SOLUBILITIES
OF
INORGANIC AND ORGANIC
SUBSTANCES
A COMPILATION OF QUANTITATIVE SOLUBILITY
DATA FROM THE PERIODICAL
LITERATURE
BY
ATHERTON SEIDELL, PH.D.
Hygienic Laboratory, U. S. Public Health
Service, Washington, D. C.
SECOND EDITION
ENLARGED AND THOROUGHLY REVISED
NEW YORK
D. VAN NOSTRAND COMPANY
25 PARK PLACE
1919
COPYRIGHT, 1907, 1911, 1919,
BY
D. VAN NOSTRAND COMPANY
Stanbope jpress
F. H.GILSON COMPANY
BOSTON, U.S.A.
PREFACE
The principal object in preparing a compilation of solubility
data, from the point of view of the advancement of chemistry, is
to furnish material for the origination and verification of theories
of solution. The majority of investigators who have been en-
gaged on such problems, have been compelled to determine ex-
perimentally the values required for developing the generalizations
they hoped to establish. In fact, a large part of the most accurate
data which are here brought together, are the outgrowth of such
studies. It is hoped, therefore, that the present effort to make
these and all other quantitative results more accessible for theo-
retical studies of solubility, will lead to noteworthy advances in
this field of chemistry.
Of the various properties which determine the uses of com-
pounds in a chemical way, solubility is of first importance. There-
fore, solubility data are perhaps of even greater interest from a
practical than from a theoretical point of view. For this reason it
has been necessary to consider the needs of those who require such
information only incidentally and may, therefore, be less familiar
with some of the forms used for its expression. With this in
mind, and at the suggestion of users of the preceding edition,
chapters have been prepared in which are described, among other
things, the sources of solubility data, the methods of calculating
them to desired terms, the interpretation of their tabular arrange-
ment, as well as some of the methods used for the accurate deter-
mination of solubilities.
Soon after the previous edition was issued, the collection of the
new data, to be used in keeping the subject matter up to date,
was systematically begun. In doing this, the experiment was
made of examining each journal page by page, instead of scan-
ning the titles of original papers contained in it. This resulted in
the discovery of many data that would otherwise have been over-
looked, and it soon became apparent that a more careful search of
the literature than that previously made was necessary. It was,
therefore, decided not only to examine the current periodicals
minutely, but to go through the back volumes in a manner equally
as thorough. The data collected in this way soon amounted to more
than could be advantageously added as a supplement to the tables
in the first edition, and it was decided to wait until the whole
book could be completely rearranged, before making any additions
iii
PREFACE
to the subject matter. It also appeared advisable to extend the
scope to include freezing-point and certain other data, which had
been omitted entirely from the first edition. The undertaking,
therefore, developed far beyond the original expectation of regu-
larly adding, from year to year, the new data which would keep
the compilation up to date. Since the amount of time at my dis-
posal for this work was limited, progress necessarily has been
slow. Finally, the advent of the war extended the period far be-
yond the limit caused by other conditions.
Although the compilation has now been completed, I realize
that in a work of this kind, more satisfactory results would have
been achieved if several individuals had cooperated in its prepara-
tion. The recent decision of the American Chemical Society to
extend its activities to the publication of reference books, will, I
hope, insure that hereafter, compilations of the present character
will be made in the exceptionally thorough manner which only an
organization with elaborate facilities can provide.
In this connection I wish to express the opinion that the new
venture of publishing compendia of chemical literature, which the
chemical societies of England and America are just now about to
undertake, will prove of service to the progress of chemistry in
English speaking countries, second only to that rendered by the
journals of original and of abstract literature, which these societies
have so successfully developed.
I realize, more than ever, that opportunities for the occurrence
of errors are innumerable and although I have endeavored to
maintain unremitting vigilance to avoid them, my efforts toward
this end have not always been successful. I desire to express my
appreciation to all who have called attention to errors in the
former edition and I will be equally grateful to those who point
out to me needed corrections in the present book. In this con-
nection, I am greatly indebted to Professor B. N. Menschutkin of the
Polytechnic Institute (Sosnovka), Petrograd, Russia, who, in calling
my attention to an error in the tabulation of some of his work
given in the first edition, sent me a complete set of reprints of his
many papers on solubility and personally corrected the tables
which I prepared from them, for use in the present volume.
In conclusion I wish gratefully to acknowledge the assistance
rendered me by Dr. W. S. Putnam of the Cooper Union of New
York during the compilation of the first 150 pages of the tables.
A. S.
WASHINGTON, D. C.,
Feb. 22, 1919.
iv
GENERAL INFORMATION
The following detailed account of the collection and arrangement
of the solubility data contained in the present volume, has been
prepared particularly for those who need quantitative solubilities
rarely, and are more or less unfamiliar with the usual tabular
methods of expressing such data. To those who are better ac-
quainted with the subject, the descriptions in some cases at least,
will probably be considered more elementary than necessary. It is
hoped, however, that with the aid of the explanations here given,
no one need remain uncertain as to the true meaning of any result
or form of expression found in the book.
Sources of the Data. — In addition to those determinations made
for the specific purpose of ascertaining particular solubilities, many
results are reported in connection with the study of theories of
solution and are, therefore, easily located. On the other hand, since
solubilities often form only an incidental part of an investigation,
many valuable data can be found only by a very careful search of
the literature. Consequently, in collecting material for the present
compilation, the procedure was adopted of perusing, page by page,
every volume of a selected number of chemical journals, for the
years 1900 to 1918. In doing this, attention was paid particularly,
to collecting all tabulated data, but a vigilant watch for solubility
statements in the text was also maintained. The twenty-three
journals which were examined in this manner are designated with
asterisks (*) in the volume-year table of journals given at the end
of the book. There is also listed in this table a somewhat larger
number of other journals, containing relatively few papers in which
solubility data may be expected. In these cases, a page by page
examination would have required more effort than the results to be
gained appeared to justify. Consequently, only the tables of con-
tents of these journals were searched for references to solubility
data. The last volume number given for each journal in this table
shows the final volume examined as above mentioned.
Of the abstract journals, only "Chemical Abstracts" was syste-
matically searched for references to data published in other than
the twenty-three journals which were minutely examined. The
original of practically all references obtained in this way was
consulted.
GENERAL INFORMATION
The larger handbooks of inorganic and organic chemistry, such
as those of Dammer, Moissan, Gmelin-Kraut, Abegg, Beilstein and
others, were not examined, since it was believed that the major part
of the data so obtained would undoubtedly have been already col-
lected from the journals.
Of the available compendia of physical constants, only the fourth
edition of Landolt and Bornstein's "Tabellen" and the three issues
of the international "Tables annuelles de Constantes et Donnees
Numerique" were systematically examined, and in these cases the
volumes were used principally to check the completeness of the
compilation made directly from the journals.
Of the various pharmacopoeias and pharmaceutical reference
books, only the eighth edition of the U. S Pharmacopoeia (1905)
was used to any extent as a source of solubility data. Most of the
results contained in the subsequent ninth edition (1916), are taken
from the previous edition and calculated to the basis of volume, in-
stead of weight, of solvent required to dissolve unit weight of solid.
It is believed that, for the present compilation, the weight basis for
expressing the results is to be preferred, and moreover, by taking
the data directly from the eighth edition, the errors incidental to
the recalculation and rounding off to whole numbers, are elimi-
nated.
In this connection, it should be mentioned that the results ob-
tained from pharmaceutical reference books for the more complex
compounds such as the alkaloids, are for the most part of only
qualitative interest, and although probably of sufficient exactness
for use in pharmaceutical compounding, do not come within the
scope of quantitative accuracy adopted for the present volume.
Collection and Compilation of the Data. — In all cases where solu-
bility results were found recorded in an original communication,
the data and accompanying descriptions of the experiments were
copied and the record thus made filed for future use. In preparing
these abstracts the actual experimental results were always recorded
when available, rather than the values as recalculated by the author
to terms which best suited the solution of the problem in hand. In
many cases the original analytical data were not given and uncer-
tainties arose as to the factors used and as to just how the calcula-
tions had been made. This was particularly true in the many cases
where the results were expressed in gram molecular quantities per
given volume of solution or on the basis of molecular percentage.
The supplementary information sought in each paper included
such points as the method which had been employed for securing
vi
GENERAL INFORMATION
equilibrium, the care exercised in purifying the material, the exact
composition of the solid phase, the procedure followed in separating
the saturated solution and analyzing it, as well as any other details
which might be of value in forming a correct estimate of the ac-
curacy of the work. The time consumed in this part of the exami-
nation of the original papers was usually found to have been well
spent when the compilation of the solubility tables from these data
sheets was undertaken. This was especially the case when it be-
came necessary to compare the results for the same compounds
obtained by two or more investigators. When practically all
abstracting of the solubility data in the journals already referred to
had been completed, the data sheets, which were at first grouped
according to the journals examined, were arranged alphabetically
in accordance with the names of the compounds for which data had
been determined. In this way all results for a particular compound
were brought together and the actual preparation of the systemati-
cally arranged tables could be begun.
It will be noted that by this plan the original papers were practi-
cally all consulted before the actual compilation of any of the data
was started. In only a small percentage of cases was the author's
paper again consulted, at the time the manuscript of the compiled
tables was prepared or later. Although this plan introduces
numerous opportunities for errors resulting from the recopying of
the original data, it appeared to be the only practical procedure.
A more direct transference of the original results to the finished page
would have required that the work be done in the library or that a
much larger number of books be withdrawn than is ordinarily
permitted.
Although it was originally intended to have the manuscript
pages typewritten before transmitting them to the printer, this
plan had to be abandoned on account of the difficulty in obtaining
the services of a competent person and also on account of the
considerable added expense. This necessity may possibly have
resulted advantageously, since one of the several opportunities for
the introduction of mistakes through copying the figures, was
eliminated.
The copy as forwarded to the printer was, for the most part,
clear and legible but it was far from the orderly character of type-
written pages, consequently, it would be surprising if none of the
many errors made by the compositors as a result of imperfect
copy, were overlooked during the proof-reading, which from be-
ginning to end was done without assistance. In order to reduce
vii
GENERAL INFORMATION
typographical and all other errors to the least possible number, it
would be necessary to compare every original paper with the final
printer's proof and to repeat every calculation of a result one or
more times. That this was not possible in the present case will
be easily realized when the very large amount of the data is
considered.
These details are mentioned at this time because it is believed
that the user of the book is entitled to exact information in regard
to the conditions under which the compilation was made. It is
only with a clear understanding of its limitations that the book
can be used to greatest advantage.
In this connection it should be pointed out that although oppor-
tunities for errors in recording the purely numerical data here
brought together are abundant, in the majority of cases the mis-
takes are not necessarily misleading if proper regard is paid to the
general import of the results as a whole. Thus on the basis of the
well-established principle that changes in solubility, such as are
due to temperature or concentration of solvent, always proceed
regularly, errors in the case of one or more figures in a table will
become apparent on careful comparison with the remaining results,
or by plotting them on cross section paper and drawing the curve.
Consequently, the table as a whole provides a check on the indi-
vidual results of which it is composed.
Scope. — In brief, it may be stated that it has been the inten-
tion to include in this compilation, the actual results, or a reference
to all quantitative solubility data, recorded in the journals referred
to in a preceding section and listed in the table at the end of the
book.
Freezing- or melting-points of binary or more complex systems,
as explained in the footnote on page I , are considered to be quanti-
tative solubility data. The experimental results are quoted for
only those systems in which one component is water or alcohol,
or which are mixtures of fairly well-known compounds, and ref-
erences are given to all others for which data were found
Owing to the uncertainty of the boundary between solubility
and other equilibria, it has been necessary arbitrarily to draw the
line in regard to certain data which it has appeared wise to exclude.
In accordance with this, no attempt has been made to gather
either figures or references, for the following:
(a) Melting-point data for mixtures of metals (alloys).
(6) Melting-point data for mixtures of minerals, except a few
of relatively simple composition,
viii
GENERAL INFORMATION
(c) Freezing-points of very dilute solutions made for the de-
termination of molecular weights or electrolytic disso-
ciation.
(d) Data for the solubility of gases in molten metals.
(e) The so-called solubility of metals in various solvents, due
to a chemical reaction which occurs.
(/) Data for solid solutions.
(g) Data for compounds of unknown or variable composition.
Order of Arrangement. — The alphabetical arrangement is be-
lieved to have the advantage that data for particular compounds
can be more easily located than would be the case if various com-
pounds- or systems had been grouped according to selected rela-
tionships. There is one difficulty which applies equally to any ar-
rangement designed to avoid duplications, and that is the placing
of those systems for which solubility results are given for two or
more of the constituents involved. This applies especially to
freezing-point lowering data for binary mixtures. In these cases
the results show in turn the solubility of each component in the
other and it is necessary to choose one, or to record the results under
the name of each member in two separate places. There are many
similar cases, in aqueous systems of two or more salts and of mix-
tures of liquids, where results are given in succession for the solu-
bility of each component in solutions of varying concentrations
of the other. In order to prevent duplication in these cases it was
necessary arbitrarily to select that component under which the
results for the entire system are to be recorded. In harmony with
the general alphabetical plan of the book, it appeared most logical
to make the selection on the basis of the alphabetical order of the
names of the compounds involved. In the majority of cases,
therefore, every system in which solubility data for two or more
compounds are given, is placed under the name of that component,
the initial of which comes earliest in the alphabet.
The advantage of this plan is that every system is assigned to a
single position by rule and opportunities for unknowingly record-
ing independent investigations of the same system, under different
headings at widely separated portions of the book, are avoided.
An exception to this rule, which it was considered wise to observe,
is in connection with mixed systems containing a compound of one
of the rarer elements. In these cases, on account of the greater
interest in the rare earth compound, the data have been located
under its name.
In the case of those mixtures of salts and liquids which yield
ix
GENERAL INFORMATION
liquid layers over certain concentrations and, therefore, to all in-
tents and purposes become reciprocally soluble liquid mixtures, they
are placed under the name of the salt or of that component which
exists as a solid under ordinary conditions. It has only rarely been
possible to give cross references in the body of the book, but in
all cases those components of the mixtures, other than the one
under which the data are alphabetically recorded, are included
in the subject index of the book and the reader, therefore, should
not fail to consult the index when results or a cross reference to
the desired compound are not found in the proper place in the
body of the book.
Nomenclature. — In regard to questions of the proper naming of
compounds for the purpose of their correct alphabetical arrange-
ment, particularly in respect to organic compounds, the usage
followed in the index of "Chemical Abstracts" Has been adopted.
Thus the name under which a given compound is indexed in
"Chemical Abstracts" is, in practically all cases, the one used for
deciding its position in the present compilation.
The most notable deviation from this rule is in the case of com-
pounds of those metals to which specific names, differing from the
name of the metal itself, have been given; thus, for example in
the present compilation, iron salts are not classed under ferrous
and ferric and tin salts under stannous and stannic but under iron
and tin, respectively. Another exception is the grouping of di
and tri substituted amines under the mono substituted compound,
instead of placing them under the widely separated headings Di
and Tri. Thus results for diethylamine and triethylamine are
given in connection with ethyl amine instead of being grouped,
on the one hand with dimethyl, dipropyl, diphenyl, etc., amines,
and on the other with trimethyl, tripropyl, triphenyl, etc., amines.
In harmony with the adoption of "Chemical Abstracts" as
authority for the correct naming of compounds, the rules adopted
for that publication (see, in connection with index to Vol. n,
1917) have been followed as closely as possible in all other matters
connected with systematic nomenclature. The exceptions which
may be found are either mistakes, or occur in those tables reused
from the first edition, in which corrections of the original plates
would have cost more than the advantage to be gained appeared
to justify. (For example, see first table, page 144, and many
others in which the old forms of spelling names such as aniline,
sulfate, glycerol, etc., have not been corrected.)
Abbreviations. — Although, in practically every case the abbre-
GENERAL INFORMATION
viations which have been used are identical with those adopted
for "Chemical Abstracts" and will, in general, be readily under-
stood, for the sake of accuracy and as a matter of convenience a
list of those made use of in the present volume is given at the
close of this chapter. (Page xxi.)
Literature References. — In order to save space, when several
references must be given in connection with one result or table,
and to avoid the repetition of the complete journal reference
when data for different compounds are given in the same paper,
an abbreviated form of reference, consisting of the name of the
author and year of the work, has been adopted. These are to be
used in connection with the author's index, in which the complete
references are arranged chronologically under each name.
Deviations from this system occur in connection with the tables
reused from the first edition. In these cases it was decided not
to incur the expense of altering the plates simply for the sake of
uniformity. The complete references given with the old tables
are sometimes, but not always, repeated in the author's index.
Forms of Stating and Methods of Calculating Solubilities to Desired
Terms. — When a solid compound is brought in contact with a
liquid, more or less of it dissolves with the production of a homoge-
neous liquid mixture. The disappearance of the solid in the
liquid continues, however, only up to a certain point, beyond
which at a given temperature, no more of the solid can be made
to dissolve. This quantity is designated as the solubility of the
compound in the particular liquid. Solubility, therefore, always
refers to a saturated solution and is expressed numerically in
terms of the composition of the homogeneous liquid in equilib-
rium with an excess of undissolved solid. It is obvious that the
composition of a saturated solution may be expressed in a great
variety of terms and it is, therefore, to be expected that investi-
gators will choose those terms which best suit the elucidation of
the particular problems in hand.
As might be expected, the terms in most general use and those
which permit of the widest applicability of the results, are based
on the weights of the ingredients of the saturated solution. These
may be either the weight of the dissolved compound contained in a
unit weight (usually 100 grams) of the homogeneous liquid mixture,
which corresponds to percentage of the dissolved compound in
the saturated solution, or else the weight of the dissolved sub-
stance in a unit weight of the solvent. In either case the one
form may be easily calculated to the other. Thus, for instance,
xi
GENERAL INFORMATION
if it is found that 100 grams of the saturated solution contain
20 grams of the dissolved compound, there can be present only
loo — 20 = 80 grams of solvent, and since this 80 grams of solvent
holds 20 grams of the dissolved compound, 20 -r- 80 X 100 = 25
grams of it are present per 100 grams of solvent. The calculation
in the opposite direction is, of course, just as simple. If 100 grams
of solvent contain 25 grams of dissolved compound, then 100 + 25
grams of solution must contain 25 grams or 100 grams of saturated
solution contain ^ X 100 = 20 grams of the dissolved compound.
In the case of most solubility statements contained in the phar-
maceutical literature, the results are given in terms of weight or
volume of solvent required to dissolve unit weight of solid. Since
all such results are simply the reciprocal of the terms, grams solid
contained in unit number of grams of solvent, the procedure for
transforming them to the more usual form simply involves dividing
I gram by the stated number of grams of solvent. In < those
cases, however, where the amount of solvent is expressed in vol-
ume instead of weight, it is first necessary to multiply by the
specific gravity of the solvent in order to find the weight corre-
sponding to the given volume.
A more serious complication is, however, introduced in those
cases where the results have been reported only in terms of vol-
ume of the saturated solution (100 cc. or I liter). On account of
the change in volume which always results when a solid dissolves
in a liquid, a calculation of the weight of the solvent present,
when only the weight of the dissolved compound and total volume
of the solution is given, cannot be made. . In these cases it is
also necessary to know the weight of a unit volume of the satu-
rated solution, that is, its specific gravity, in order to convert
the results from the volume to the weight basis. Consequently,
for solubility results to be most generally useful, the specific gravity
of the saturated solution should always be determined.
The calculation of a given result from the volume to the weight
basis or vice versa, with the aid of the specific gravity (density),
is readily understood when it is remembered that this factor is
simply the weight in grams of I cc. of the solution. If, for example,
it is stated that 100 cc. of saturated solution contain 25 grams of
salt and the specific gravity is 1.15, it is apparent that 115 grams
of the solution contain 25 grams of the salt, or 100 grams contain
— £- =21.7 grams. Conversely, when the calculation of the
amount of salt in 100 cc. from that in 100 grams of solution, is to
xii
GENERAL INFORMATION
be made, the weight of dissolved compound must be multiplied
by the specific gravity.
One of the forms of presenting solubility data for which especial
care is needed in converting the values to a different basis is in
the case of results for salts with water of crystallization. In some
instances these results are expressed in weight of the hydrated
compound in a given volume or weight of the saturated solution.
If it is desired to ascertain the weight of anhydrous salt present,
it will be necessary first to calculate the grams of anhydrous salt
equivalent to the stated number of grams of the hydrated com-
pound and, if the results have been expressed in terms of volume
of saturated solution, this will be all that is necessary, but if, for
instance, the grams of hydrated salt per 100 grams of saturated
solution or of water have been given, then it will be necessary to
add the weight of water present as water of crystallization in the
salt, to the weight of water present as solvent. The total weight
of solvent is, therefore, made up of the weight of water used for
preparing the solution and that carried by the salt as t^O of
crystallization.
In the case of solvents composed of mixtures of water and alcohol,
or other liquids, authors sometimes fail to specify whether the
figures for such mixtures refer to the weight or volume basis,
consequently, without a specific gravity determination, the exact
composition of the mixture is uncertain. The above remarks con-
cerning the calculation of solubility results from one form to another
apply equally to determinations made in mixed solvents, provided
all supplementary data for accurately establishing the composition
of the mixed solvent are given.
Although in most cases the actual experimental results of solu-
bility determinations are obtained in terms of weight, many investi-
gators find that certain advantages are to be gained, in particular
problems, by converting their analytical results to the basis of
normality or gram molecules, and in practically all such cases it is
not thought necessary to present also the gram quantities from
which the molecular values were calculated. Although this may
be justified from the narrow point of view of the particular problem
in hand, it is greatly to be deplored when the broader aspects of the
value of solubility data as a whole are considered. As already
mentioned, solubility results which have been determined for some
one purpose may frequently be applied to the solution of other
problems, or serve in the development or testing of generalizations
or of laws of solution. It is, therefore, important that in the case of
xiii
GENERAL INFORMATION
all solubility data the results should either be expressed in the
gravimetric terms derived most directly from the experimental de-
terminations, together with the specific gravities of, and solid phases
in contact with the solutions, or else, when presented in terms more
or less remote from those of the directly determined values, the
method of making the calculations should be plainly indicated and
all factors or supplementary data which have been used, presented
in detail.
In preparing the present compilation occasion was several times
taken to write to authors for data supplementary to those published,
which although not essential to the solution of the particular prob-
lem in hand, and therefore omitted from the paper, were, neverthe-
less, needed for calculating the results to a form which would permit
comparison with similar data by others or their use in the solution
of other problems.
The calculation of results from the molecular basis to the gram
basis or vice versa, introduces, in addition to the errors incidental
to the calculation itself, those resulting from the selection of the
atomic or molecular weights which are used as the factors. It is
indeed rare for an author to state the actual molecular weights used
for a calculation, and although the revisions of atomic weights
which are occasionally made are usually not of great magnitude,
opportunities for slight differences in recalculating results to a
desired basis, due to differences in molecular weights, are worthy of
consideration. A source of greater inaccuracies, however, is that
resulting from the failure of authors to differentiate clearly between
the significance of normality (gram equivalents) and gram molecules
(formula weights) in calculating or in expressing their results.
It also occasionally happens that the compounds involved are de-
scribed only by names which are not specific and a doubt may arise
as to the exact formula expressing the composition of the compound
in question. This applies particularly to work described in lan-
guages other than English. In cases of complex mixtures of several
salts the results are sometimes given in terms of the ions present
and the calculation of such results to the gram basis calls for especial
care.
The general procedure for calculating gram quantities to the
molecular basis consists simply in dividing by the molecular weight,
or molecular equivalent weight in the case of results to be expressed
in normality, and pointing off according to the unit quantity of
solution selected. The reverse calculation is, of course, made by
multiplying the molecular or normality values as given, by the
xiv
GENERAL INFORMATION
molecular, or molecular equivalent weights. An example which
will illustrate the principal points involved, is the case of the calcu-
lation of the grams of dissolved compound per 100 grams of solvent,
from a result expressed in terms of molecular per cent, that is, in
terms of molecules of dissolved compound present in a total of 100
molecules of dissolved compound plus solvent. Thus, in the case
of the solubility of mercuric iodide in pyridine, it has been found
that the saturated solution at 100° contains 25 mol. per cent HgI2,
which designates a mixture of 25 gram mols. of HgI2 and 100 — 25
= 75 gram mols. of pyridine. To convert to gram quantities, each
figure is multiplied by the respective molecular weight and the
product for the HgI2 divided by the product for the C5H5N. Thus,
(25 X 45445) •*• (75 X 79.08) = 1.915, which, X 100, = 191.5
grams HgI2 per 100 grams of C6H5N.
Although, in the present compilation an attempt has been made
to calculate as many as possible of the data to terms of weight of
the compounds involved, especially for the commoner substances,
this has not appeared advisable in some cases, either on account of
uncertainties as to the factors to be used, or on account of the rela-
tive unimportance of the data and the considerable labor which
would have been involved in making the calculations.
The principal terms used in expressing the solubility of gases in
liquids are defined in connection with the tables of data in the body
of the book. See, for instance, p. 227.
Explanation of Tables. — Although the tables of results contained
in the present volume will, it is hoped, be easily understood by all
who are familiar with the subject, for the benefit of those who need
solubility data only rarely, it has appeared desirable to mention
some of the principles followed in constructing the tables and ex-
plain in detail the exact meaning of the results contained in a num-
ber of typical tables.
The main consideration in connection with a compilation such
as the present one, is to arrange the very large amount of material
in the most concise manner compatible with perfect clearness. It
has, therefore, been necessary to adopt forms and abbreviations
which eliminate the repetition of readily understandable details.
In general, it may be stated that the record of a solubility de-
termination consists of the analytical results showing the composi-
tion of a homogeneous liquid mixture in equilibrium at a given
temperature, with one or more solid compounds or with another
homogeneous liquid mixture. In the case of aqueous solutions of
salts, for instance, the analysis will show the weight of salt and of
xv
GENERAL INFORMATION
water contained in a given amount of the saturated solution. In
recording this analysis, however, as solubility data, it is not cus-
tomary to state the weight of water directly, since its quantity is
derivable from the given weight of salt and of solution (salt plus
water). Thus, in all cases the amount of the dissolved compound
is numerically reported in terms of unit quantity (100 grams, one
liter, etc.) of the saturated solution or of the solvent. The tables,
therefore, all show in the heading above the columns of figures, the
terms in which the results are expressed (grams, cubic centimeters,
gram molecules, etc.) and the unit quantity of solution or solvent
in which the numerically recorded amounts of dissolved compound
are contained. When more than one column of figures are inclosed
under a bracket below the heading, the arrangement is an abbrevia-
tion designed to eliminate the repetition of the heading over each
column separately, and, therefore, indicates that the heading applies
independently to each separate column of figures. Thus, in the
case of the table showing the solubility of sodium nitrate in water
(see p. 656) the heading which is as follows:
Cms. NaN03^per 100 Gms. j^ols
Solution. Water. ' per Liter.
o 42.2 72.9-73* 6.71*
10 44.7 80.8-80.5 7.16
when translated into its detailed meaning shows, (i) that at o°, 100
grams of the saturated solution of sodium nitrate in water contain
42.2 grams NaNO3, (2) that at o°, 100 grams of water dissolve from
72.9 to 73 grams NaNOs according to the authorities quoted
(Mulder or Berkeley), and (3) that one liter of a saturated solution
of sodium nitrate in water at o° contains 6.71 gram molecules of
NaNO3.
This general form of heading is typical and will be found in prac-
tically all cases where results for the solubility of a single salt in a
single solvent at various temperatures are given. As will be noted,
tables of this form show the results for a single series of determina-
tions at increasing temperatures expressed in more than one set of
terms. As a general rule, and especially when determinations of
the specific gravities of the solutions are also given, any one of the
figures for a given temperature may be calculated, as described in
the previous section, from either of the others at the same tempera-
ture. The advantages of tables giving the results in several sets of
terms are that the reader is relieved of making the calculations
individually.
xvi
GENERAL INFORMATION
In a number of cases where, either the importance of the com-
pound does not warrant very detailed results, or where similar data
for several near related compounds have been determined, com-
posite tables showing the results for two or more compounds in one
or more solvents have been constructed. Although by this pro-
cedure considerable space has been saved and frequent repetitions
avoided, it is possible that clearness has sometimes been sacrificed.
An example of such a composite table is that for the three com-
pounds, CdI2.KI.H2O, CdI2.2KI.2H2O and CdI2.2NaI.6H2O given
in the first table on p. 178. The three solvents in which the
solubilities were separately determined are placed in the first
column of the table. Next follow the results for CdI2.KI.H2O,
given in terms both of grams of anhydrous salt, CdI2.KI, per 100
grams of solution and per 100 grams of solvent. The next group of
figures shows successively the solubility of CdI2.2KI.2H2O in water,
in absolute alcohol and in absolute ether, reported in each case, in
terms of grams of anhydrous salt per 100 grams of saturated solution
and also in grams per 100 grams of each solvent. The last group of
figures, columns 6 and 7, gives similar results for CdI2.2NaI.6H2O.
Other examples of this type of table are given on p. 188. In
these cases results for three compounds, each in the same solvent
but at different temperatures, are given. The abbreviation here
adopted consists in providing only one column of temperatures to
serve for each of the three sets of results given in the succeeding
columns. This general plan is followed in a very large number of
cases throughout the book.
One other example is that of the results for platinic double
chlorides, given in the first table on p. 498. In this case, although
each column of results represents an independent series of solubili-
ties in water, they have all been grouped under the same bracket,
instead of each being given under a separate, complete heading.
By this plan a very compact arrangement has been provided but the
results are apt to be misunderstood unless the reader bears in mind
that here as elsewhere it has been necessary to condense the data
as much as possible.
Before leaving the general subject of composite tables, attention
should be called to one point which will be found illustrated in a
large number of them. This is in reference to results at other tem-
peratures than those which apply to the table as a whole, as recorded
in the first column under the designation t°. In these cases the
figure for the temperature is given in a parenthesis immediately
following the result for grams of compound dissolved and, of course,
xvii
GENERAL INFORMATION
means that the particular determination was made at the tem-
perature stated in the parenthesis, instead of at the temperature
shown in the column t°, which applies to all the results not so
modified.
This principle of indicating in parentheses any variations from
the general order of the table, and also in respect to the introduction
of additional matter, such as results for densities, points on the
character of the solutions, etc., is one which has been followed in
many instances.
As already stated, a solubility is an expression of the con-
centration of a solution in equilibrium with a particular solid com-
pound. Therefore, if a compound can exist in more than one form
at a given temperature, such as in different states of hydration, its
solubility will show variations in accordance with which one of its
forms is in contact with the saturated solution at the particular
temperature. Information in regard to the solid phase is, conse-
quently, essential to the accurate expression of a solubility. When-
ever such facts are available they are shown in the tables by means
of formulas recorded under the heading "Solid Phase." These
formulas are usually placed on a line with the numerical results for
the solution in contact with the solid represented by the formula
given.
A case which illustrates strikingly the multiplicity of variations
in solubility with change in degree of hydration is that of the solu-
bility of the hydrates of ferric chloride in water (see p. 337). In
this case, to economize space, the formula for the hydrate has been
placed immediately above that group of data to which each refers,
instead of on the same line with the results for each solution in
contact with that particular hydrate. An examination of this table
will show the apparent anomaly that the same hydrate possesses
two different solubilities at certain temperatures. Thus, in the
section of the table giving results for solutions in contact with the
solid phase Fe2Cl6.i2H2O, it will be noted that 100 grams of H2O
dissolve 106.8 grams FeCla at 30° and two lines below, the same
amount of water is stated to dissolve 201.7 grams FeCl3 at 30°.
This is due to the fact that each of the hydrates gives a more or less
well developed reverse solubility curve. The character of these
curves is plainly indicated by plotting them on cross-section paper
from the results given in the table. If this is done it will be seen
that in case of the results for Fe2Cl6.i2H2O, the grams of FeCl3 con-
tained in 100 grams of water increase regularly with rise of tem-
perature up to 37°, which is the melting-point of this hydrate. If
xviii
GENERAL INFORMATION
more crystals are added and the temperature raised above 37°, they
melt and form a homogeneous solution of increased concentration.
K, however, this more concentrated solution is cooled again below
37°, and crystals then added, they remain as solid phase and, when
equilibrium is established, the composition of the solution corre-
sponds to a point on the upper, reverse arm, of the solubility curve.
With this salt, therefore, it is seen that for certain ranges of tem-
perature the concentration of the saturated solution depends upon
the procedure by which the point of equilibrium has been ap-
proached.
In cases where results are given for the solubility of a particular
compound in aqueous solutions of another, the heading above the
columns of figures shows, as usual, the terms in which the results
are expressed (gms., cc., mols., etc.) and the unit amount of solution
or solvent in which the recorded amounts of each compound is con-
tained; while below the bracket are given, at the heads of the
columns, the formulas of the respective compounds simultaneously
present in the solution. Thus, there will usually be found in one
column, the increasing concentrations of the salt present in the
aqueous solution constituting the solvent, and in the other the
amounts of the other compound of which the solubility is being de-
termined and which is present as solid phase in contact with the
solution. Examples of this form of table are those for the solubility
of calcium sulfate in aqueous salt solutions (pp. 215 to 219) and
numerous others throughout the book. In all cases where the solid
phase exists in more than one form, this information, when available,
is recorded in the usual manner in the column under the heading
"Solid Phase." (See pp. 174, 185, 203, 404, and many others.)
The results for the specific gravities of the saturated solutions are
also given, when available. It is needless to say that, according to
the arrangement of these tables, the figures in the horizontal lines
refer to the same solution and those in the vertical columns to dif-
ferent solutions of the series.
In the case of tables showing the distribution of a compound
between two immiscible solvents (see for example, results for mer-
curic chloride, pp. 420 and 421), the amounts of the dissolved com-
pound in the conjugate layers are given under the same bracket
with column headings designating the respective layers. In the
case of equilibria in ternary systems, which form two liquid layers
(see for example, last table, p. 511), the compositions of the upper
and lower layers are given under separate brackets, the results on
each horizontal line being for layers in contact with each other.
xix
GENERAL INFORMATION
Data of this character are described more fully in the chapter on
Methods for the Determination of Solubility.
The types of cases which have just been described were pointed
out by users of the first edition of the book who did not understand
the arrangement in these cases and suggested that an explicit de-
scription of them would make the book more generally useful. It
is realized that the explanations which have been given here apply
only to a certain proportion of the tables in the book. There are,
no doubt, many tables and forms of expression, especially for the
more complex systems, which will not be understood by the casual
reader. In some of these cases brief remarks in connection with
the tables have been given, but to just what extent these explanatory
remarks are warranted, it has been difficult to decide. In conclu-
sion, it should be mentioned that the title of the table is intended
to describe the nature of the results and should always be used as a
guide in the interpretation of the tabular arrangement.
xx
ABBREVIATIONS
Most of the following abbreviations will be found written both with capitals
and without.
WD- — Specific Rotation.
abs. — Absolute.
abs. coef . — Absorption Coefficient.
alcohol. — Ethyl Alcohol.
amt(s). — Amount (s).
anhy. — Anhydrous.
aq. — Aqueous.
atm(s). — Atmosphere(s).
at. wt. — Atomic Weight.
b.-pt. — Boiling-point.
C. — Centigrade.
calc. — Calculate (ed).
cc. — Cubic Centimeter (s).
cm. — Centimeter (s).
coef. — Coefficient.
com. — Commercial.
compd. — Compound.
cone. — Concentration, Concentrated.
cond. — Conductivity.
const. — Constant.
cor. — Corrected.
crit. — Critical.
cryo. — Cryohydric.
cryst. — Crystalline.
d. — Dextro (in connection with the
name of an optically active com-
pound).
d. — Density (dis — Specific Gravity
at 1 8°, referred to water at 4°; d^
at 20° referred to water at 20°),
decomp. — Decomposition.
dif. — Different.
dil. — Dilute.
dist. coef. — Distribution Coefficient.
ed. — Edition.
elec. — Electric (al).
equil. — Equilibrium.
equiv. — Equivalent (s).
eutec. — Eutectic.
F. — Fahrenheit.
f.-pt. — Freezing-point.
g., gm., gms. — Gram(s).
gm. mol. — Gram Molecule (s).
G. M. — Gram Molecule (s).
hr(s). — Hour(s).
i. — (d + /) Inactive (in connection
with the name of an optically active
compound.)
inorg. — Inorganic,
insol. — Insoluble.
/. — Laevo (in connection with the
name of an optically active com-
poun4).
kg. kgm. — Kilogram (s).
1. — Liter(s).
mm. — Millimeter (s)
m. — Meta.
max. — Maximum,
mg., mgm. — Milligram(s).
mol(s). — Molecule(s), Molecular,
mol. wt. — Molecular Weight,
millimol. — Milligram Molecule,
m.-pt. — Melting-point.
n. — Normal (gm. equiv. per 1.).
N. — Normal (used rarely).
o. — Ortho.
ord. — Ordinary,
org. — Organic,
p. — Page.
p. — Para,
pet. — Petroleum,
ppt. — Precipitate,
pt. — Point.
quad. pt. — Quadruple Point,
qual. — Qualitative,
sapon. — Saponification.
sat. — Saturated,
sol(s). — Solution (s).
sp. gr. — Specific Gravity (Density),
sq. cm. — Square Centimeter.
s. — Symmetrical,
sym. — Symmetrical.
xxi
ABBREVIATIONS
fc°. — Temperature, Centigrade- Scale. wt. — Weight.
temp(s). — Temperature (s). oo — Infinity.
tr.pt. — Transition Point. .lo"2, .io~5, etc., following a result
vol(s). — Volume (s). means that the decimal point is to be
undissoc. — Undissociated. moved as many places to the left as
U. S. P. — U. S. Pharmacopoeia, indicated by the minus exponent.
XXll
ACENAPHTHENE C12Hi0.
SOLUBILITY IN SEVERAL ORGANIC SOLVENTS.
(Speyers — Am. J. Sci. [4] 14, 294, 1902.)
NOTE. — In the original paper the results are given in terms of gram mole-
cules of acenaphthene, acetamide, acetanilide, etc., per 100 gram molecules of
solvent, at temperatures which varied with each solvent and with each weigh-
ing of the solutions. The tabulated results here given were obtained by re-
calculating and reading the figures from curves plotted on cross-section paper.
In Methyl Alcohol. In Ethyl Alcohol. In Propyl Alcohol.
t °. (a)
(ft)
(c)
(a)
(ft)
(c) •
"(a)
(ft)
(0 "
0
81
•33
I
.80 o
•39
81.1
1.9
0.57
82.3
2.26
0.88
10
80
.40
I
.70 o
•38
80.3
2.8
0.84
8l.8
2.40
i .00
2O
79.60
2
.25 o
.48
79.6
4.0
1.20
81.4
3-40
!-35
30
79
.00
3
.50 o
.72
79.1
5-6
1.70
80.9
4-75
i .90
40
78
•45
6
.00 I
.20
78.7
8.4
2.6o
80.6
7.10
2.90
50
78
•15
9
.00 I
•77
78.8
13.2
3-90
80.7
II. 10
4.40
60
78
•30
ii
.70 2
•35
79-4
23.2
7.00
81 .5
19.60
8.20
70
78
.60
14
.30 2
.90
80.75
40-5
12.50
83-9
37.00
16.20
In Chloroform.
In Toluene.
t °.
(a)
(ft)
(c)
<«)
(ft)
(c)
0
143-8
16.
4 12-7
90.7
I3.I8
7-9
10
I40.I
20.
6 16.0
90.8
18.0
10.7
20
I36-3
27.
o 19.5
91.0
24-5
14-5
30
132.4
34-
o 25 .0
91.8
33-5
20.5
40
128.0
42.
5 32-0
92-7
47.0
28.0
50
123.4
Si-
5 40.0
94.0
60.5
35-7
60
119.3
62.
5 5°-°
95-5
74.0
43-5
70
.
97.2
89.0
52-5
(a) Weight of 100 cc. solution in grams. (b) Grams dissolved substance per 100 grams solvent.
(c) Gram molecules of dissolved substance per 100 gram molecules of solvent.
looo gms. Aq. 25% NH3 dissolve 0.07 gm. acenaphthene at 25°. (Hilpert, 1916).
RECIPROCAL SOLUBILITIES DETERMINED BY THE METHOD OF LOWERING OF THE
FREEZING-POINT * ARE GIVEN BY GIUA (1915), FOR THE FOLLOWING PAIRS
OF COMPOUNDS:
Acenaphthene + m Dinitrobenzene.
+ 2.4 Dinitrotoluene.
" + a. Trinitrotoluene.
• Freezing or Melting-point Curves as Solubility Data. — When a mixture of two compounds, rendered
liquid by elevation of temperature, is gradually cooled, a point will be reached at which one or the other
of the constituents will separate as a solid. This point represents the solubility of the one compound in
the other. The method involved, differs principally from that ordinarily employed for solubility de-
terminations, in that the composition of the mixture remains constant while the saturation tempera-
ture is being approached, instead of the reverse procedure.
A considerable amount of data of this character is available, but, after careful consideration, it has
been decided that references only will be given to it in the present volume, except in cases of mixtures
of well-known compounds or of those in which water is one of the constituents.
RECIPROCAL SOLUBILITIES (Freezing-point Lowering Data, see footnote, page i )
ARE GIVEN FOR THE FOLLOWING PAIRS OF COMPOUNDS:
Acenaphthene + Chloroacenaphthene
-j- Bromoacenaphthene
" -|- lodoacenaphthene
+ Benzil
-j- p Nitrobenzoic Aldehyde
" + Piperonilic Aldehyde
+ Vanillic Aldehyde
Chloroacenaphthene + Bromoacenaphthene
+ lodoacenaphthene
Bromoacenaphthene -j- "
(Crompton and Walker, 1912.)
(Pawlewski, 1893.)
(Fazi, 1916.)
(Crompton and Walker, 1912.)
ACETALDEHYDE CH3COH.
SOLUBILITY IN ETHYL ALCOHOL DETERMINED BY THE METHOD OF LOWERING
•OF FREEZING-POINT (de Leeuw, 1911). Liquid air was used as the cooling
medium and temperatures were measured with the aid of a specially con-
structed resistance thermometer.
-123-3
-125.4
— 127.6
-132
-126
-126
-124.3
-123.5
Wt.
Per Cent
CH3COH
in
Mixture.
Mol.
Per Cent
CH3COH
in
Mixture.
100
ICO
90.7
84.5
80.9
78.1
90.3
83-9
80.2
77-3 '
75-2
67.0
60.8
74-4
66.0
59-7
Solid Phase.
r.
CH3COH —122.3
-I25-3
-128
(Eutectic) —123.2-
77.3 CH3COH.C2H5OH —126.8
-130.6
— 120.6
-II4.9
Wt. Mol.
Per Cent Per Cent
CH3COH CH3COH Solid Phase.
in in
Mixture. Mixture.
51.8 50.7 CH3COH.C2H5OH
45-6 44-5
40.6- 39.5 CH3COH.2C2H5OH
35-3 34-3
30.2 29.3
17.9 17.3 C2H6OH
10.2 Q.8
o.o o.o
Freezing-point data for mixtures of acetaldehyde and paraldehyde as well
as the complete x — T diagrams are given by Holleman (1903). Results for
mixtures of paraldehyde and p xylene are given by Paterno and Ampola (1897).
Results for mixtures of the a and /3 forms of Acetaldehyde phenyl hydrazone
are given by Laws and Sidgwick (1911).
AOETAMIDE CH3CO.NH2.
SOLUBILITY IN WATER AND IN ALCOHOL.
(Speyers.)
In Water.
In Ethyl Alcohol.
t°.
(«0
(ft)
(c)
' (a)
(ft) («)"
0
105
•5
70
.8
29
.6
85
.62
J7
•3
18.5
10
104
•9
81
.0
34
• o
86
.2
24
.0
26.0
20
104
•3
97
•5
40
.8
87
3
31
.5
33-8
30
103
•7
114
.0
47
•7
88
.8
40
•5
43-0
40
103
.0
133
.0
55
•5
90
•7
5o
.0
S3 -5
50
102
•3
154
.0
64
.0
93
.0
61
.0
60
101
.6
177
•5
74
• 0
95
5
72
• o
76S
1 (a) Wt. of 100 cc. sat. solution in gms.
Acetamide per 100 gm. mols. solvent.
100 gms. pyridine dissolve 17.75 gms. acetamide at 20-25°; Io° gms. aq. 50 per
cent pyridine dissolve 84.7 gms. acetamide at 20-25°. (Dehn, 1917.)
Freezing-point curves are given for: Acetamide + Benzene (Moles and
Jimeno, 1913); Acetamide + Phthalide (Lautz, 1913); Acetamide + Triphenyl
guanidine (Lautz, 1913); Tribromoacetamide + Trichloroacetamide (Kiister,
1891).
ACETANILIDE
ACETANILIDE C6H6NH.COCH3.
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent.
Water
Ether
Formic Acid (95%)
Acetic Acid (99.5%)
Acetone
Amyl Acetate
Amyl Alcohol
Aniline
Benzene
Benzaldehyde
Toluene
Xylene
Pyridine
50% Aq. Pyridine
Petroleum Ether
i6
25
30
25
21-5
30^31
25
30-31
25
32.5
20-25
u
about 20
0-997
i .000
1. 121
O.9O2
0.882
1.034
0-875
1.068
0.862
0.847
0-47
0-54
0.69
2.8
56.74
33-21
10.46
14.00
19.38
2.46
18.83
0.50
1.65
32.7
35-7
0.03
Authority.
(Greenish and Smith, 1903.)
(Holleman and Antush, 1894.)
(Seidell, 1907.)
(Marden and Dover, 1916.)
(Aschan, 1913.)
(Seidell, 1907.)
(Dehn, 1917.)
(Salkower, 19x6.)
SOLUBILITY IN METHYL ALCOHOL, ETHYL ALCOHOL AND IN CHLOROFORM.
(Speyers, 1902.) See Note, page i.
In CH3OH.
O
10
20
30
40
50
60
Sp. Gr. of
Sat. Solu-
tion.
0.860
0.864
0.875
0.892
O.9II
0.932
0.957
Gms.
C8H5NH.COCH,
per zoo Gms.
Sat. Solution.
18-5
23.1
29.1
35-i
42.9
5!-7
59-2
In
C2H5OH.
Sp. Gr. of
Sat. Solu-
Cms.
C6H5NHCOCH3
per too Gms.
tion.
Sat. Solution.
0.842
12.8
0.844
16.7
0.850
21.3
0.860
26.5
0.874
32.9
0.895
39-4
0.920
46.4
In CHCV
Sp. Gr. of
Sat. Solu-
tion.
Gms.
CeHjNHCOCHa
per 100 Gms.
Sat. Solution.
I-503
3-53
1-475
7.24
1.440
10.7
1.398
14-5
1-354
18.7
1.3*4
23-7
1.272
29.1
SOLUBILITY OF ACETANILIDE IN MIXTURES OF ETHYL ALCOHOL AND WATER.
wt.
nesuiis at 25 . \r\
Loiieman ana /wuusn, 1094.;
K.CSUILS at j
50 . v^e'ueu, 1907.;
lerCent
:2H5OH in
Solvent.
Sp. Gr. of Sat.
Solution.
Gms. C6H6NH.COCH3
per too Gms. Sat.
Solution.
Sp. Gr. of Sat.
Solution.
Gms. C6HSNH.GOCH,
per loo Gms. Sat.
Solution.
0
0.997
o-54
I .OOO
0.69
10
0.985
0-93
0.984
I.QD
2O
0-973
1.28
0.970
2.20
30
0.962
2.30
0.956
4.80
40
0.950
4-85
0-945
9.40
50
0-939
8.87
Q-934
15.40
60
0.928
14.17
0.926
22.00
70
0.918
19.84
0.917
27.60
80
0.907
25-I7
0.907
31.20
85
0.899
26.93
0.900
31.70
00
0.890
27.65
0-893
51.60
95
0.874
26.82
0.885
30.80
IOO
0.851
24-77
0.876
29.OO
(See remarks under a Acetnaphthalide, page 13.)
ACETANILIDE 4
SOLUBILITY OF ACETANILIDE" IN MIXTURES OF ETHER AND CHLOROFORM AND OF
ACETONE AND BENZENE AT 25°. (Marden and Dover, 1916.)
Results for Ether-Chloroform Mixtures. • Results for Acetone-Benzene Mixture.
Wt Per Cent C H Gms' C6H5NH.COCH3
Wt. .rer l^ent ^srls __ /-• n/r:»«j
Wt. Per Cent CHC13
in Mixed Solvent.
Gms. C6H5NH.COCH3
per 100 Gms. Mixed
Solvent.
100
17.7
90
80
II.7
8.2
70
00
6.2
4-95
50
40
4-25
3-8
30
3-5
20
3-25
10
3-05
0
2.9
100 1.36
90 6.78
•80 13.0
70 20.0
60 29.2
50 30.0
40 3°-5
30 33-o
20 36.0
10 45-7
o ' 39-4
DISTRIBUTION OF ACETANILIDE BETWEEN IMMISCIBLE SOLVENTS AT 25°.
Cone. C6H5NH.COCH3 in Benzene layer -f- Cone, in H2O layer = 1.65.
(Farmer and Warth, 1904.)
" Chloroform " -r- Cone, in H2O layer = 7.75.
(Marden, 1914.)
" Ether " -f- Cone, in H2O layer = 2.98.
(Marden, 1914.)
SOLUBILITY OF HALOGEN SUBSTITUTED ACETANILIDES IN ETHYL ALCOHOL AT
DIFFERENT TEMPERATURES. (Chattaway and Lambert, 1915.)
Gms. of Each Anilide per 100 Gms. of Each Sat. Solution.
t°.
p Chloro-
acetanilide.
2.4 Dichloro-
acetanilide.
p Bromo-
acetanilide.
2.4 Dibromo-
acetanilide.
4 Chloro-
2 Bromo-
acetanilide.
2 Chloro-
4 Bromo-
acetanilide.
5
4.244
2.480
. . .
. . .
10
3.278
3.008
4.847
2.876
4-334
2-575
15
3-777
3-564
5-56I
3-382
5.088
2.961
20
4.366
4.192
6.390
4.002
5.986
3.466
25
5.040
4.962
7.300
4.714
7-043
4-095
30
5.828
5.864
8.440
5-6I5
8.328
4.891
35
6.700
6-937
9-7I5
6.686
9.844
5.820
40
7.728
8.276
11.156
7.914
11.586
6.887
45
8.918
9-750
12.767
9-357
13.718
8.186
(Results for unstable needle forms of p bromoacetanilide and 2.4 dibromo-
acetanilide are also given.)
SOLUBILITY OF p NITROACETANILIDE AND OF 2.4 DICHLOROACETANILIDE IN
ACETIC ACID AT l6°. (Orton and King, 1911.)
Compound. Solvent. <5SS£&SR
p Nitroacetanilide Glacial Acetic Acid o . 83
50% Aq. " 0.38
2.4 Dichloroacetanilide Glacial Acetic Acid 6.37
50% Aq. " 0.83
Freezing-point curves (see footnote, page i) are given for mixtures of:
Acetanilide and Antipyrine (Comanducci, 1912.)
' m Nitraniline ' (Crompton and Whiteley, 1895.)
" m Dinitrobenzene "
' a Dinitrophenol
" p Nitroacetanilide (Kiister, 1891.)
p Nitroacetanilide and Dinitroacetanilide (Holleman and Sluiter, 1906.)
p Bromoacetanilide and 2.4 Dibromoacetanilide (Sidgwick, 1915.)
ACETIC ACID
ACETIC ACID CH3COOH.
RECIPROCAL SOLUBILITY OF ACETIC ACID AND WATER DETERMINED BY THE
METHOD OF LOWERING
OF THE
FREEZING-POINT
.
Gms. CH3COOH
Gms. CH3COOH
t°.
per 100 Gms. Solid Phase.
Sat. Solution.
t°.
per 100 Gms.
Sat. Solution.
Solid Phase.
o
o Ice
— 2O
67.0
CH3COOH
- 5
15-2
— 15
72.3
"
— 10
28.5
— 10
77-5
"
"~I5
40.0
- 5
82.2
it
— 20
49.2
0
87.0
it
— 25
K
+ 5
91.8
tt
-26.
7 60 . o (Eutectic)
10
95-8
it
-25
62.5 CH3COOH
16.6
100. 0
ft
The data in the above table were obtained by plotting the results of Pickering
(1893), Roloff (1895), Dahms (1896) (1899), deCoppet (1899), Kremann (1907),
Faucon (1910), Ballo (1910), Groschuff (1911), Paterno and Salimei (1913), and
Tsakalotos (1914), on cross-section paper and drawing a curve through the points
in best agreement. In addition to making determinations of the freezing-points
of the mixtures, Ballo also analyzed the solid phases which separated, and snowed
that these contained, in all cases, increasing percentages of acid and, therefore,
must have consisted of mixed crystals. This formation of mixed crystals is
offered as an explanation of the abnormality of the freezing-point lowering of
the system.
SOLUBILITY OF ACETIC ACID IN ETHYL ALCOHOL (98.9%) DETERMINED BY
THE METHOD OF LOWERING OF FREEZING-POINT. (Pickering, 1893.)
Gms. CH3COOH
Gms. CH3COOH
t°.
per zoo Gms.
Sat. Solution.
Solid Phase.
-75
26.O
CH3COOH
-70
27.7
tt
-60
33-o
it
-So
38.2
ft
-40
43-7
tt
-30
50.2
tt
— 20
58.0
ft
t°.
per too Gms.
Sat. Solution.
Solid Phase.
— 10
67.7
CH3COOH
- 5
73-2
n
0
79.1
tt
+ s
85.2
tt
10
Qi-5
ft
15
98.0
tt
16.6
IOO.O
tt
(The original results were plotted on cross-section paper and the above figures
read from the curve.)
SOLUBILITY DATA DETERMINED BY THE METHOD OF LOWERING OF THE FREEZ-
ING-POINT (see footnote, page i) ARE GIVEN FOR MIXTURES OF Acetic Acid
AND EACH OF THE FOLLOWING COMPOUNDS:
Chloroacetic Acid (Mameli and Mannessier, Dimethyl pyrone (Kendall, 1914 (a).)
. J9I3: Kendall, 1914.)
DlchloroacetlC Add (Kendall, 1914.)
Tnchloroacetic Acid (Kendall, 1914.)
Acetic Anhydride (Pickering, 1893.)
Booge, 1916.)
Benzene + Vaseline (Roloff, 1895-)
Benzene + Naphthalene (Roloff, 1895.)
Benzene + Water (Roloff, 1895.)
Benzoic Acid (Kendall, 1914.)
Chlorobenzene (Baud, 1913 (c).)
Nitrobenzene (Dahms, 1895; Baud, 1913 (c).)
Carbon Disulfide (Pickering, 1893.)
Cyclohexane (Baud, 1913 (a) (6).)
Dimethyl Oxalate (Kendall and Booge, 1916.)
Dimethyl Succinate (Kendall and Booge, 19x6.)
Eth j Ether (Pickermg> l893.}
Ethylene Bromide (Dahms.tSgs; Baud, I9i2(a).)
Ethylene Dibromide (Baud, *'„ (>,)
tormamide (English and Turner, 1915.)
Formic Acid (Baud, 1913 (c).)
Methyl Alcohol (Pickering, 1893.)
Picric Acid (Kendall, 1916.)
Propyl Alcohol (Pickering, 1893.)
Sulfuric Acid (Pickering, 1893.)
Thymol (Paterno and Ampola, 1897.)
p Xylene (Paterno and Ampola, 1897.)
ACETIC ACID 6
DISTRIBUTION OF ACETIC ACID BETWEEN:
Water and Amyl Alcohol at 20°. Water and Benzene at 25°.
(Herz and Fischer, 1904.) (Herz and Fischer, 1905.)
Cms. CHaCOOH G. M. CHaCOOH Cms. CH8COOH G. M. CHaCOOH
per IPO cc. per 100 cc. per 100 cc. per 100 cc.
H20 Alcoholic' HsO ' Alcoholic" H^O C6H6 ' TlzO C6H6 "
Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer.
1 0.923 o-oi 0.0095 5 0.130 0.05 0.0014
2 1.847 °-°3 0-0280 io 0.417 o.io 0.0005
3 2.741 0.05 0-0460 20 i-55 0.20 0.0030
4 3-694 0.07 0.0645 30 3-03 0.30 0.0290
5 4-587 0.09 0.0830 40 4.95 0-50 0.051
6 5-475 o-11 o.ioio 0.70 0.090
7 6.434 0.13 0.1190
8 7.328
NOTE. — The distribution results of Herz and co-workers are reported in
millimolecules per io cc. portions of each layer in the several cases. To obtain
the figures given in the tables here shown, the original results, before and after
calculating to gram quantities, were plotted on cross-section paper, and from
the curves thus obtained, readings for regular intervals of concentration of
acetic acid in the aqueous layer were selected.
DISTRIBUTION OF ACETIC ACID BETWEEN WATER AND BENZENE.
(Waddell, 1898; see also Lincoln, 1904.)
The measurements were made by adding varying amounts of benzene or water
to 5 cc. of acetic acid and then running in water or benzene till saturation was
reached. The observed readings were calculated to grams per 100 grams of the
liquid mixture.
Upper Layer. Lower Layer.
t°. CHaCOOH. C6H6. 5^6. CHaCOOH. CeH6. H&T
25 0.46 99-52 0.02 9.4 0.18 90.42
25 3-10 96.75 0.15 28.2 0.53 71.27
25 5.20 94-55 °-25 37-7 °-84 61.46
25 8.7 90.88 0.42 48.3 1.82 49.88
25 16.3 82.91 0.79 61.4 6.1 32.5
25 30-5 67.37 2.13 66.0 13.8 20.2
25 52-5 39-6o 7-60 52.8 39.6 7.6
35 1.2 98.68 0.08 16.4 0.62 82.98
35 5-7 93-97 °-33 36-8 1.42 62.78
35 9-° 90.42 0.58 49 -o 2.10 48.90
35 45.0 49-0° 6.0 61.3 25.5 13.2
35 52-2 39.4 8.4 52.2 39.4 8.4
Additional data in connection with the distribution of acetic acid between
water and benzene are given by King and Narracutt (1909), Kuriloff (1898),
Farmer (1903), Bubanovic (1913), and Lincoln (1904). This latter investigator
points out that the same degree of clouding does not represent the end point in
all cases as was assumed by Waddell (1900).
Data for the distribution of acetic acid between benzene and aqueous solu-
tions of sodium acetate at 25° are given by Farmer (1903).
ACETIC ACID
DISTRIBUTION OF ACETIC ACID BETWEEN WATER AND CHLOROFORM:
At Room Temperature. At 25°.
(Wright, Thomson and Leon — Proc. Roy. (Herz and Lewy; Rothmund and Wilsmore.)
Soc. 49» 185, 1891.)
Results in parts per 100 parts of solution.
Upper Layer. Lower Layer.
Cms. CHaCOOH
per TOO cc.
G. M. CHgCOOH
per 100 cc.
CHaCOOH. CHCla-
H2O. CHsCOOH
. CHC13.
H20.
H20
Layer.
CHC13
Layer.
H20
Layer.
CHCI;
Layer.
O
0.84
99
.16
o
99.01
0.99
2
o.
089
0.05
0.0032
6.46
0.92
92
.62
1.04
98.24
0.72
4
O.
3i3
0.075
0.0062
17.69
0.79
81
•52
3.83
94.98
I.I9
6
o.
596
0.100
O.OIOO
25.10
I. 21
73
.69
6.77
91.85
1.38
8
o.
974
0.150
0.0198
33 7i
2-97
63
•32
11.05
87.82
I-I3
10
I.
43°
0-175
0.0260
44.12
7-30
48
•58
17.72
80.00
2.28
12
I.
982
0.200
0.0325
50.18
15.11
34
•7i
25-75
70.13
4.12
20
5-
10
0.30
0.070
30
10.2
0.50
O.I7O
40
15-
3
O.70
0.275
50
21.
9
0.80
o-335
52-3
39-
54
0.87
0.659
See Note, page 6.
In addition to the above results, data for somewhat lower concentrations of
acetic acid determined at 20° are given by Dawson and Grant (1901).
Results showing the influence of electrolytes upon the distribution of acetic
acid between water and chloroform are given by Rothmund and Wilsmore and
by Dawson and Grant.
DISTRIBUTION OF ACETIC ACID AT 25° BETWEEN:
Water and Carbon Disulphide.
(Herz and Lewy.)
Cms. CHsCOOH
G. M. CHsCOOH
per ipo cc.
per 100 cc.
H20 CS2'
H2O CS2"
Layer. Layer.
Layer. Layer.
65 2.64
I.I 0-45
7O 3-O
1.2 0.55
75 3-3
1.2 0.80
80 5.4
i-35 0.97
85 6.4
1.4 1.3
Water and Carbon Tetrachloride.
(Herz and Lewy.)
Cms. CH3COOH G. M. CH3COOH
per IPO cc.
per 100 cc.
H20
Layer.
30 1.8 0.5 0.03
40 3.0 0.7 0.055
50 4.8 0.9 0.095
60 5.8 i.i 0.155
7O 12. 0 1.2 0.235
76.2 25.2 1.27 0.420
Results for the distribution of acetic acid between water and mixtures of
equal volumes of carbon disulfide and carbon tetrachloride at 25° are given
by Herz and Kurzer (1910)*
DISTRIBUTION OF ACETIC ACID AT 25° BETWEEN:
ecu
Layer.
Water and Bromoform.
(H. and L. — Z. electro. Ch. ix, 818, '05.)
Cms. CHaCOOH G. M. CHaCOOH
Water and Toluene.
(H. and F. — Ber. 38, 1140, '05.)
Cms. CH3COOH -G. M. CH3COOH
per 100 cc.
per ipo cc.
H20
Layer.
CHBr3
Layer.
'H20
Layer.
CHBr3
Layer.
20
I .5
0-4
0-035
30
3-o
0.6
0.070
40
4-8
0.8
0.120
50
7.8
i -o
O-2O
60
12.0
i .1
0.28
65
I5.6
1.15
o-395
70
27.0
per ipo cc.
per 100 cc.
H2O C6H5CH3
Layer. Layer.
H2O
Layer.
C6H5CH3
Layer.
5 Q-II9
O.I
0.0025
10 0.328
0.2
0.0075
20 I-I32
0-4
O.O26O
30 2.265
0.6
0.0530
40 3-725
0.8
0.090
50 5.841
i.o
0.140
60 8.344
See Note, page 6.
ACETIC ACID 8
DISTRIBUTION OF ACETIC ACID BETWEEN WATER AND ETHYL ETHER.
(de Kolossovsky, 1911.)
Results at Several Temperatures.
Gms. CH3COOH per 100 cc. of:
H2O
Ether
P
Layer (p).
Layer (p').
P''
13
0.365
0.207
I.76
18
0.367
O.2OI
1.82
27
0-379
0.195
1.94
7-5
0-799
0.551
I .45
12
0.803
0.529
1.52
18
0.802
0.501
1. 60
25
0.789
0.474
1.66
Results at 18°.
Gms. CHgCOOH per 100 cc. of:
H20
Ether
p
Layer (p).
Layer (p').
p''
1.0
0.5 i
l.O
2.0
1.0 J
2.0
4.0
2.1 ]
•9
6.0
3-5 3
•7
8.0
4-9 J
.6
10. 0
6.6
•5
15-0
EX.4
•3
20. o
17.0
.2
25.0
23-3 :
[.07
According to results obtained at 25° by Morgan and Benson (1907), the ratio
of distribution for concentrations of acetic acid up to 12 grams per 100 cc. of
the H2O layer is more nearly constant (1.92) than shown above for 18°. A
similar constancy of distribution (approx. 2.08 at 15°) was also found by Pinnow
(1915)-
Results showing the influence of varying concentrations of a large number of
electrolytes upon the distribution of acetic acid between water and ether are
given by de Kolossovsky, Dubrisay (1912), and by Hantzsch and Vagt (1901).
Data for the distribution of acetic acid between ether and molten CaCl2.6H2O
and ether and molten LiNO33H2O are given by Morgan and Benson (1907).
One determination of the distribution of acetic acid between sat. aq. CaCl2
solution (20 gms. per 1.) and kerosene gave 97.7 gms. acid per 100 gms. aq. layer
and 27 gms. per 100 gms. kerosene layer at ordinary temperature. (Crowell,
1918.)
DISTRIBUTION OF ACETIC
Water and o or p Xylene.
(Herz and Fischer.)
ACID AT 25° BETWEEN:
Water and m Xylene.
(Herz and Fischer.)
Gms. CH3COOH
per 100 cc.
G,
, M. CH3COOH
per 100 cc.
Gms. CH3COOH
per 100 cc.
G
. M. CH3COOH
per 100 cc.
IT r» o or p
l52. X*lene
Layer.
H20
Layer.
o or p TT Q m
Xylene L vr X^ene
Layer. y ' Layer.
H2O
Layer
m
Xylene
Layer.
C O
.24
O
.1
O
.004
5
0
.06
0
.1
0.0015
IO O
.48 ,
0
.2
0
.010
IO
0
•30
0
.2
O.OO7
20 I
.13
O
•4
0
.025
20
0
•95
O
•4
O-O22
30 2
mI5
o
.6
0
.047
30
I
.91
o
.6
0.042
40 3
.40
o
.8
0
.079
40
3
.04
o
.8
0.072
50 5
.10
I
.0
0
.122
50
4
•65
I
.0
O.III
60 7
.27
I
.2
0
.230
60
6
•65
I
.2
...
70 12
•52
»•
See Note, page 6.
Data showing effect of camphor on the reciprocal solubility of acetic acid and
olive oil are given by Wingard, 1917.
ChloroACETIC ACIDS
ChloroACETIC ACIDS CH2C1COOH, CHC12COOH, and CCUCOOH.
SOLUBILITY OF THE a, ft, AND 7 MODIFICATION OF MONOCHLORO ACETIC Aero
IN WATER AT DIFFERENT TEMPERATURES.
(Miers and Isaac, 1908; Pickering, 1895.)
The determinations were made by the sealed tube method. The following
figures were obtained by plotting the original results on cross-section paper:
Cms. per 100 Gms. of Each Sat.
Solution.
Gms. per 100 Gms. of Each Sat.
Solution.
a 'Modifi-
/3 Modifi-
7 Modifi-
t .
cation.
cation.
cation.
20
...
. . .
88.0
25
. . .
85.8
90.0
30
86.0
88.2
92.2
35
88.4
90.6
94.1
40
90.8
93-9
95-8
45
93-o
95-o
97.8
*o a Modifi-
0 Modifi-
•y Modifi-
cation.
cation.
cation.
50
95
.0
97
.0
99
.6
51
(m. pt.)
.
.;
100
.0
55
97
.2
99
• 3
.• t
.
56
.5 (m.pt.)
,
too
.0
.
60
99
.0
t
.
62
.4 (m. pt.)
0:00
.0
. .
. .
, .
, •
Reciprocal solubilities of mono-, di-, and trichloroacetic acids and water de-
termined by the freezing-point method are given by Pickering (1895).
SOLUBILITY OF TRICHLQROACETIC ACID IN WATER AT 25°.
(Seidell, 1910.)
100 gms. saturated solution of d& = 1.615 contain 92.32 gms. GC13.COOH.
SOLUBILITY DATA DETERMINED BY THE METHOD OF LOWERING OF THE FREEZ-
ING-POINT (see footnote, page i) ARE GIVEN FOR MIXTURES OF Chloro-
acetic Acid AND EACH OF THE FOLLOWING COMPOUNDS:
Dichloroacetic Acid (Kendall, 1914.)
Trichloroacetic Acid (Kendall, 1914.)
Acetophenone (Kendall and Gibbons,
Dibenzyl Acetone (Kendall and Gibbons, 1915.)
Benzil (Kendall and Gibbons, 1915.)
Benzene (Kendall and Booge, 1916.)
Benzoic Acid (Kendall, 1914.)
Camphor (Pawlewski, 1893.)
Cinnamic Acid (Kendall, 1914.)
Crotonic Acid
Cetyl Alcohol (Mameli and Mannessier, 1913.)
0 Cresol (Kendall, 1914.)
Methyl Cinnamate (Kendall and Booge, 1916).
Dimethyl Oxalate (Kendall and Booge, 1916.)
Dimethyl Succinate (Kendalland Booge, 1916.)
Dimethylpyrone (Kendall, 1914 (a).)
Naphthalene (Miers & Isaac, 1908; M. & M.,i9i3.)
Phenol (Kendall, 1916.)
Piperonal (Kendall &Gibbons, I9IS;M.&M.,I9I3.)
Salol (Mameli and Mannessier, 1913.)
Sulfuric Acid (Kendall and Carpenter, 1914.)
0 Toluic Acid (Kendall, 1914.)
m "
p " "
a "
Vanillin (Kendall and Gibbons, 1915.)
SOLUBILITY DATA DETERMINED BY THE METHOD OF LOWERING OF THE FREEZ-
ING-POINT (see footnote, page i) ARE GIVEN BY KENDALL (1914) FOR MIX-
TURES OF Dichloroacetic Acid AND EACH OF THE FOLLOWING COMPOUNDS:
Trichloroacetic Acid
Benzoic Acid
Cinnamic Acid
Crotonic Acid
Dimethylpyrone
o Toluic Acid
m "
p " "
a "
(Phenylacetic Acid)
ChloroACETIC ACID
10
SOLUBILITY DATA DETERMINED BY THE METHOD OF LOWERING OF THE FREEZ-
ING-POINT (see footnote, page i) ARE GIVEN FOR MIXTURES OF Trichloro-
acetic Acid AND EACH OF THE FOLLOWING COMPOUNDS:
(Kendall and
Gibbons,
I9IS-)
AcetOphenone (Kendall and Gibbons, 1915.)
Anisaldehyde
Benzene (Kendall and Booge, 1916.)
Benzaldehyde (Kendall and Gibbons, 1915.)
m Hydroxy Benzaldehyde
p "
o Nitro Benzaldehyde
m "
p "
Benzophenone
Benzil '
Benzoquinone
Benzoic Acid (Kendall, 1914.)
Camphene (Timofeiew & Kravtzov, 1915, 1917.)
Cinnamic Acid (Kendall, 1914.)
Crotonic Acid
0 Cresol (Kendall, 1914.)
Diethyl Oxalate (Kendall and Booge, 1916.)
Diethyl Succinate
Dimethyl Oxalate
Dimethyl Malonate
Dimethyl Succinate
Dimethyl Terephthalate (Kendall and
Booge, 1916.)
Dimethylpyrone (Plotnikov, 1911; Kendall,
1914 (o)-)
Ethyl Ether (Tsakalotos and Guye, 1910.)
Ethyl Acetate (Kendall and Booge, 1916.)
Ethyl Benzoate " "
Methyl Benzoate
Anisate
" Cinnamate " "
" />Toluate
a Naphthol (Kendall, 1916.)
0 "
a Naphthyl Acetate (Kendall and Booge, 1916.)
a « « ((
P
Phenol (Kendall, 1916.)
o Nitro Phenol (Kendall, 1916.)
m "
p " "
Piperonal (Kendall and Gibbons, 1915.)
Nitro Piperonal
Phenyl Anisylketone "
" Benzoate (Kendall and Booge, 1916.)
" Salicylate " "
Salicylic Aldehyde (Kendall and Gibbons.igis.)
Sulfuric Acid (Kendall and Carpenter, 1914.)
0 Toluic Acid (Kendall, 1914.)
m "
p " "
a " " "
Thymol (Kendall, 1916.)
Vanillin (Kendall and Gibbons, 1915.)
DISTRIBUTION OF CHLORACETIC ACID BETWEEN:
(Herz and Fischer.)
Water and Benzene at 25°.
Water and Toluene at 25°.
Cms. CH2C1COOH
G. M. CH2C1COOH
Cms. CH2C1COOH
G. M. CH2C1COOH
per zoo cc.
per i po cc.
per 100 cc.
per 100 cc.
HaO C*He'
Layer. Layer.
Layer. Layer.
H20 QHsCfta
Layer. Layer.
620 CeHsCHs
Layer. Layer.
0.25* 8.69
O.OO25 0.090
o.i* 5.22
o.ooi 0.055
o-S 15-59
O.OO5 0.155
0-5 20.31
O.OO5 O.2O
1.0 27.87
o.oio 0.28
i.o 34.87
o.oio 0.36
1.5 41.10
0.015 0.415
1-5 49.14
O.OI5 0.50
2.0 52.90
O.O2 0-54
2.O 60.46
O.O2 O.62
3.0 68.01
O.O3 0.70
3-0 72.28
0.03 0-77
40 76.52
O.O4 O-79
4-0 81.72
O.O4 0.85
5.0 86.94
0.05 0.90
* See Note, page 6.
Additional data for the distribution of monochloroacetic acid between water
and benzene as well as similar results for dichloroacetic acid are given by
Georgievics, 1915.
II
ChloroACETIC ACIDS
DISTRIBUTION or CHLORACETIC ACID BETWEEN:
(Herz and Lewy.)
Water and Chloroform at 25°. Water and Bromoform at 25°.
Cms. CH2C1COOH
G. M. CH2C1COOH
Cms. CH2C1COOH
G. M. CHaClCOOH
. per
100 CC,
per 100 cc.
per 100 cc.
per 100 cc.
H20
Layer.
CHC13
Layer.
1H20
Layer.
CHC13
Layer.
H2O
Layer.
CHBr3
Layer.
H2o
Layer.
CHBrs
Layer.
5*
0.283
0.05
0.0025
40*
0.850
0-45
O-OII
10
0.6l4
o.io
O.OO6O
So
1.889
0.50
0.0165
20
1. 088
O.2O
O.OI3S
60
2.994
O.6o
O.O28
40
2.948
O.4O
O.O29
70
4.241
0.70
0.040
50
3.684
0-6o
0.045
80
5.620
0.8o
0-053
60
4.440
0.70
0.061
90
7.560
0.90
0-067
70
7.086
o-75
0.077
91 .6
11.340
0-97
0.120
DISTRIBUTION OF CHLORACETIC ACID BETWEEN:
(Herz and Lewy.)
Water and Carbon Disulphide
at 25°.
Water and Carbon Tetra-
chloride at 25°.
Cms. CHzClCOOH
per 100 cc.
G
. M. CH2C1COOH
per 100 cc.
Cms. CH2C1COOH
per 100 cc.
G
. M. CH2C1COOH
per 100 cc.
'H20
Layer.
CS2
Layer.
H20
Layer.
CS2
Layer.
H2O
Layer.
ecu
Layer.
"l^O
Layer.
ecu
Layer.
60*
0
.426
O
.6
0
.0042
90*
I.4I7
0
•95
0.0150
80
0
.691
O
.8
O
.007
95
2.031
I
.00
0-0195
90
O
.803
I
.0
0
.009
100
2.645
I
•05
0-0270
100
I
.040
I
•05
O
.0105
«>5
4.26
I
.10
0.0415
105
I
.464
I
.10
0
.015
106.7
5-19
I
•13
0.0550
106.7
I
.890
I
•13
O
.020
* See Note, page 6.
Results showing the influence of sulfuric acid upon the distribution of mono-
chloroacetic acid between water and ethyl ether at 26° are given by Hantzsch
and Vagt (1901).
CyanoACETIC ACID CH2(CN)COOH.
DISTRIBUTION OF CYANOACETIC ACID BETWEEN:
(Hantzsch and Sebalt, 1899.)
Water and Ethyl Ether.
Cms. CH2(CN)COOH per
Liter.
• •
H20
(G>H ) O
Layer.
Layer.
O
0.070
0.042
10
0.076
0.044
21
0.083
0.030
30
0.089
0.027
Water and Benzene.
Cms. CH2(CN)COOH per
Liter.
6
25
H20
C,H9
Layer.
Layer.
0.067
0.02O
0.130
O.OIQ
PhenylACETIC ACID 12
PhenylACETIC ACID (« Toluic Acid) CH2(C«H5)COOH.
SOLUBILITY IN WATER AND IN ALCOHOLS. (Timofeiew, 1894.)
Gms.CH2(C6H5)COOH Cms.
Solvent. t°. per 100 Gms. Solvent. t°.
CH2(C«H5)COOH
per 100 Gms.
Sat. Sol.
Sat. Sol.
Water 20
1.64
Ethyl Alcohol o.o
50-7
Methyl Alcohol —17
50.6
+ 19-4
64.4
-13
S3-2
20.0
65.1
" o
59-2
Propyl Alcohol —17.0
29.4
+ 19-4
70.8
-13-0
32.3
" 20
71.8
0.0
40.9
Ethyl Alcohol -17
39-7
+19.4
56.8
-13
4i.5
20.0
57-2
SOLUBILITY OF PHENYLACETIC ACID IN SEVERAL SOLVENTS AT 25°.
(Herz and Rathmann, 1913.)
Gms. Gms.
Solvent. CH2(C6H5)COOH Solvent. CH2(C6H5)COOH
per 100 cc. Sat. Sol. per 100 cc. Sat. Sol.
Chloroform 60.17 Tetrachlorethylene 21.19
Carbon Tetrachloride 25.07 Tetrachlorethane 61.45
Trichlorethylene 44-89 Pentachlorethane 44.26
The freezing-point curve (Solubility, see footnote, page i) is given by Sal-
kowski (1885) for mixtures of phenylacetic acid and hydrocinnamic acid.
ACETIC ACID ESTERS.
SOLUBILITIES OF SEVERAL ACETIC ACID ESTERS IN AQUEOUS ALCOHOL AT ROOM
TEMPERATURE. (Pfeiffer, 1892.)
~. TTfV, i cc- HjjO added to cause separation of a second phase in mixtures of the given
Alcohol m amounts of Alcohol and 3 cc. of:
Mixtures.
3
6
9
12
IS
18
21
24
27
30
33
ChloroACETIC ACID ESTERS.
SOLUBILITY OF MONOCHLOR, DICHLOR, AND OF TRICHLORACETIC ESTER
IN AQUEOUS ALCOHOL AT ROOM TEMPERATURE."
(Bancroft — Phys. Rev. 3, 193, 1895-06, from results of Pfdffcr, Z. physik. chem. 9, 469, *9a.)
CH3COOCH3. CH3COOC2HS.
CH3COOC3H7.
CH3COOC4H0.
CHsCOOCgHu.
00 6.0
4-50
2.08
I.76
... °o
10.48
6.08
4.24
... ...
17.80
10.46
9-°3
... ...
26.00
15.37
13.24
... ...
35.63
20.42
I7-52
... ...
47-5°
26.60
22.22
... ...
58.71
3J-49
26.99
... ...
00
37.48
32.14
... ...
. . .
43-75
37.23
... ...
. . .
50-74
42.06
... ...
59-99
48.41
cc. Ethyl
Alcohol in
cc. H2O added to cause separation of a second phase
in mixtures of the given amts. of Alcohol and 3 cc. of:
Mixtures.
CHaClCOOCzHs.
CHC12COOC2H5
CC13COOC2H4.
3
1-32
0.90
0.65
6
4.01
2-45
1. 80
9
7-30
4-33
3.02
12
10.78
6.60
4.50
IS
16.16
9.20
6.50
18
22.16
• • •
21
28.74
• • •
• • •
13 ACETIN
Mono-, Di-f and Tri ACETIN C3H6(OH)2(OC2H8O), C3H5(OH)(OC2H3O)2, and
Trie partition coefficients of these three compounds between olive oil and
water are given by Baum (1899) and Meyer (1901, 1909), as 0.06, 0.23, and 0.3
respectively.
MethACETIN (p Acetanisidine, or p oxymethylacetanilide) C6H4.OCH8.
NHCHaCO.
100 gms. H2O dissolve 0.19 gms. of the compound at 15° and 8.3 gms. at 100°.
(German Pharmacopoeia.)
a ACETNAPHTHALIDE C2H3ONH(CioH7).
SOLUBILITY IN MIXTURES OF ALCOHOL AND WATER AT 25°.
(Holleman and Antusch — Rec. trav. chim. 13, 289, 1894.)
Vol.%
Alcohol.
Gms. per
100 Gms.
Solvent.
Sp. Gr. of
Solutions.
Vol.%
Alcohol.
Gms. per
100 Gms.
Solvent.
Sp. Gr. of
Solutions.
100
4-02
0.7916
65
I.78
0.8977
95
4-31
0.8150
60
1-44
0.9091
90
4.II
0.8344
55
I -O2
0.9201
85
3-69
0.8485
5o
0-71
0.9290
80
3.l8
0.8624
35
0.25
Q-9537
75
2-73
0.8761
20
O.O9
0.9717
70
2.31
0.8798
10
O.O4
0.9841
Constant agitation was not employed. The mixtures were allowed to stand
in bath and the solutions analyzed after different lengths of time. Formulas
are not given. This applies to all determinations by Holleman and Antush.
ACETONE (CH3)2CO.
SOLUBILITY OF ACETONE AT 25° IN AQUEOUS SOLUTIONS OF:
Electrolytes. Non-Electrolytes.
(Bell — J. Phys. Ch. 9, 544, 1905; Linebarger — Am. Ch. J. 14, 380, 1802.)
Gms. Electro-
lyte per
100 Gnis* AQ<
Gms. (CH3)2CO per 100 Gms. Gms. Non- Gms. (CH3)2CO per 100 Gms.
Solvent in Solutions of: Electrolyte Solvent in Solutions of:
Solution.
K2C03
Na2CO3
(NH4)2CO3 MgCO3" Xq. Solution. CioHat
Anethol* (C6H6)2CO
I
•25
.
83-5
5
92
•5
103.0
90.0
2
•50
51.0
IIO.O
65.0
10
117
.0
123.0
108.5
5
-CO
65'
o
38.0
73-5
47-o
20
137
.0
144-5
126.0
7
•5
46,
5
27-5
57-o
38.0
30
148
•5
155-0
i33-o
10
.0
34
5
19-5
44-5
29.0
40
155
•5
162 -O
136.0
12
•5
25
5
14.0
35-o
50
159
•5
166.0
135-5
15
.0
18
o
9-0
28.0
60
160
.2
165.0
I3I-5
20
• O
8
0
2-7
70
155
• O
158.0
123.0
25
.0
3
7
80
. i
108.5
30
.0
i
6
...
90
.
82.0
* Anethof = p Propenylanisol, CH3.CH:CH.C6H4OCH3. f Naphthalene results at 35°.
NOTE. — In the case of the results for the aqueous solutions of electrolytes,
the determinations were made by adding successive small quantities of acetone
to the mixtures of given amounts of water and electrolyte, and noting the point
at which a clouding, due to the separation of a second phase, occurred. In the
case of the aqueous non-electrolyte solutions, successive small amounts of water
were added to mixtures of known amounts of acetone and the non-electrolyte.
In all cases the results, as given in the original papers, have been recalculated
and plotted on cross-section paper. From the curves so obtained, the above
table was constructed.
Additional data for systems containing acetone are given under the salt involved,
as, for instance, Potassium Carbonate, p. 51 1, Potassium Fluoride, p. 534. etc.
ACETONE 14
MlSCIBELITY OF ACETONE AT O° WITH MIXTURES OF:
Chloroform and Water (Bonner, 1910).
Bromobenzene and Water (Bonner, 1910).
Gms.
Gms. Gms.
Sp. Gr. of
Gms.
Gms.
Gms.
Sp. Gr. of
CHClj.
H20. (CHa)2CO.
Mixture.
C«H5Br.
H20.
(CH3)2CO.
Mixture.
0.988
O.OI2 O.5OI
z.i8
0.977
0.023
0.685
1. 12
0.900
O.IOO
.300
1. 01
0.90
O.IO
I .13
1. 01
0.792
0.208
.633
0.98
0.80
O.2O
I.4I
0.98
0.696
0.304
• 750
0.96
0.70
0.30
1.52
0.97
0.600
O.4OO
.770
0.95
0.60
0.40
i-S7
0.96
0.500
0.500
.720
0.94
0.50
0.50
i .60
°-95
*O.42O
0.580
.650
*°-49
0.51
i. 60
0.400
O.6OO
.630
o-93
0.40
0.60
i-59
0.94
0.300
0.700
-530
0.94
0.30
0.70
i-55
o-93
O.2OO
0.800
.321
°-95
0.20
0.80
1.46
o-93
O.IOO
o . 900 i . 144
0.97
0.10
0.90
1.30
o-93
O.OlS
0.982 0.464
0.98
, O.O2
0.98
0.849
o-95
NOTE. — The determinations were made by gradually adding acetone to the
mixtures of the given amounts of water and the other constituent until a homo-
geneous solution was obtained. The results give the binodal curve for the sys-
tem. The author also determined "tie lines" showing the compositions of the
various pairs of liquids which may exist in equilibrium. When the two layers
are practically of the same composition the tie line is reduced to a point desig-
nated as the "plait point" of the binodal curve. This point is indicated by a *
in the above tables.
SOLUBILITY OP ACETONE IN AQUEOUS SOLUTIONS OF CARBOHYDRATES.
(Krug and McElroy — J. Anal. Ch. 6, 184, '92; Bell — J. Phys. Ch. 9, 547. '05.)
In Aqueous Solutions of Cane Sugar.
Gms. (CH3)2CO per 100 Gms. Sugar Solution at:
Percent
Sugar.
10
20
30
35
40
45
50
55
60
65
70
In Aqueous Dextrose Solutions.
15°.
20°.
25°.
30°.
35°.
40°.
597-2
581.8
574-8
272.5
250.0
251.8
172.4
150.0
150.6
no
96.4
92.8
89.8
85
. . .
71.9
68.8
65-7
. . .
62
50.8
48.1
45-9
42
...
35-8
33-8
32-5
....
29
25.2
24.2
23-4
. . .
18-3
17.7
17.0
• • •
13-2
12.8
12-5
...
In Aqueous Maltose Solutions.
Per
cent
Gms. (CH3)2CO per 100 Gms.
Solvent at:
Per
cent
Gms.
(CH3)2CO per
Solvent at:
too Gms.
Dextrose.
15°.
25°.
35°. '
Maltose.
15°
25°.
35°."
10
736
•7
747-9
761-5
10
353
.6
348
.1
342
• 0
20
255
•3
247-7
240.8
20
185
•4
181
.2
I76
•9
30
157
•5
149.8
142.5
30
119
•9
116
• O
112
•4
40
86
•9
79.6
74-o
40
78
•4
74
•7
70
•5
50
36
.2
33-o
31.2
50
46
.2
42
9
39
.8
*/ IS \J%J \J \J S \J S
The determinations were made as in the case of the solubility of acetone in
aqueous solutions of electrolytes. See preceding page.
ACETONE
DISTRIBUTION OF ACETONE BETWEEN:
Benzene and Water.
Results at 20°. Results at 25°.
(Philip and Bramby, 1915-)
Gm. (CH3)2CO per 1000 cc.
' H^O C6Hg
Layer.
0.08
Layer.
O.IO
0.20
0-30
O.40
0.12
0.25
0-34
(Herz and Fischer, 1905.)
Cms. (CH3)2CO per 1000 cc.
C6H6
Layer.
12.0
41-7
IOI.5
Toluene and Water.
At Different Temps.
(Hantzsch and Vagt, 1901.)
Cms. (CH;j)2CO per 1000 cc.
H20
Layer.
50
100
150
200
155-9
225.0
See Note, page 6.
*°
H20
Layer.
C6H5CH3
Layer.
0
2.105
0-993
10
20
30
2.000
1.960
1.867
0-957
0-957
0-957
Philip and Bramby also give data for the effect of NaCl, KC1 and LiCl upon
the distribution of acetone between benzene and water.
In the determinations by Hantzsch and Vagt the equilibrium was approached
from above. The amount of acetone in the lower layer was determined by
analysis, and that in the upper layer calculated by difference.
Water and
Carbon Tetrachloride.
Mols. (CHs)2CO per Liter.
CC14
DISTRIBUTION OF ACETONE BETWEEN:
(Herz and Rathmann, 1913.)
Water and
Chloroform.
Mols. (CH,)2CO per Liter.
H20
Layer.
0.186
0.322
1. 01
1.66
2.87
Layer.
0.0833
0.146
0.514
0.997
2.10
' H20
CHC13
Layer.
Layer.
0.032
0.168
0.0781
0-399
0.145
0.676
0.263
1.17
0-493
1.98
1. 01
3-o6
Water and
Pentachlorethane.
Mols. (CH3)2CO per Liter.
H20
Layer.
O
144
271
541
806
149
QHC16
Layer.
0.251
0.469
0.859
1-275
I-763
Water and
Tetrachlorethane.
Mols. (CH3)2CO per Liter.
Water and
Tetrachlorethylene.
Mols. (CH3)2CO per Liter.
H20
Layer.
0.249
0.317
0.363
0.569
C2H2CU
Layer.
0.341
0.994
I. 210
I-323
1.936
H20
Layer.
CC)2:CCI2
Layer.
0.081
0.274
0.562 0.174
1.020 0.343
1.545 0.629
2.007 0.891
The distribution coefficient of acetone between olive oil and water is given by
Meyer (1901), as 0.146 at 3° and 0.235 at 30°.
^ Water and
Trichlorethylene.
Mols. (CH3)2CO per Liter.
Layer.
0.160
0.350
0.654
0.946
CHCl:CCla
Layer.
0.193
0-359
0.719
1.029
1.562
SOLUBILITY DATA DETERMINED BY THE METHOD OF LOWERING OF THE
FREEZING-POINT (see footnote, p. i) ARE GIVEN FOR MIXTURES OF Acetone
AND EACH OF THE FOLLOWING COMPOUNDS:
(Maass and Mclntosh, 1912.)
Phenol
Resorcinol
Pyrogallol
(Schmidlin and Lang, 1910.)
Bromine
Chlorine
Hydrobromic Acid
Chloroform (Tskalotos and Guye, 1910.) Pyrocatechol
0 Chlorophenol (Bramby, 1916.)
Depression of the freezing-point of mixtures of acetone and water and each of
the following compounds are given by Waddell (1899): Ether, hydroquinone,
phenol, p nitrophenol, salicylic acid.
ACETOPHENONE 16
ACETOPHENONE CH3COC6H6.
The freezing-point curve for mixtures of acetophenone and sulfuric acid is
given by Kendall and Carpenter (1914).
Freezing-point curves (solubility, see footnote, page i) for mixtures of Cinna-
mylidene Acetophenone and each of the following compounds are given by
Giua (1916): Acenaphthene, azobenzene, ethyl ether and a trinitrotoluene.
ACETYLACETONE CH3COCH2COCEL
SOLUBILITY IN "WATER.
(Rothmund — Z. phys. Ch. 26, 475, '98.)
Cms. CH3COCH,COCHS per 100 Cms.
to H2O Acetyl Acetone
Layer. Layer.
30 15-46 95-02
40 17.58 93.68
50 20.22 91.90
60 23.23 89.41
70 27.10 85.77
80 33-92 78.82
87.7 (crit. temp.) 56.8
NOTE. — Weighed amounts of water and acetyl acetone were placed in small
glass tubes, which were then sealed and slowly heated until the contained mix-
tures became homogeneous. The temperature was then allowed to fall very
gradually and the point noted at which cloudiness appeared. This point was
accurately established for each tube by repeated trials. The curve plotted from
these determinations shows two percentage amounts of acetyl acetone which
cause cloudiness at each temperature below the critical point. Of these two
points, for each temperature, one represents the aqueous layer, i.e., the solu-
bility of acetyl acetone in water; and the other represents the acetyl acetone
layer, i.e., the solubility of water in acetyl acetone. This method is known as the
'Synthetic Method," and yields results in harmony with those obtained by the
analytical method, i.e., by analyzing each layer after complete separation occurs.
See also, chapter on Methods of Solubility Determinations.
ACETYLENE C2H2.
SOLUBILITY IN WATER.
(Winkler; see Landolt and Bernstein's Tabellen, 3d ed. p. 604, '05.)
t°. a. q.
O 1-73 0.20
5 x-49 o-1;
10 1.31 0.15
15 i-iS °-I3
20 1.03 O°I2
25 0.93 o.n
30 0-84 0.09
a, "Absorption Coefficient," = the volume of gas (reduced to o° and 760
mm. pressure) taken up by one volume of the liquid at the given temperature
when the partial pressure of the gas equals 760 mm. mercury.
q, "Solubility," = the amount of gas in grams which is taken up by 100 grams
of the pure solvent at the given temperature if the total pressure, i.e., the partial
pressure of the gas plus the vapor pressure of the liquid at the absorption tem-
perature, is 760 mm.
17 ACETYLENE
SOLUBILITY OF ACETYLENE IN WATER, AQUEOUS SOLUTIONS OF ALKALIES AND
SULFURIC ACID AT 15°.
(Billitzer, 1902.)
Aq. Solution
of:
Ba(OH)2
Ca(OH)2
NH4OH
NaOH
KOH
Na2S04
H2S04
SOLUBIL
/150f
Acetylen
e in Aq. Sol
utions
ot
Norma
lity:
O.OI
1.230
1.216
1. 210
1. 212
ITY IN
0.025
1.218
0.05
O.IO
1.230
0.15
1.240
0.25
0.50
1. 00
2.OO
3-oo
WATER
I.2OO
, /15 =
1.218
I.lSo
1.185
I.I70
I.I90
I.25L
I.22O
... I.I28
I.I30
. . . 1.068
1.225
1.040
1.056
0.940
I.I2O
1.230
0.885
0.912
0.720
1.040
1-235
0.6OO
0.660
0.340
0.900
1.240
0.370
0.460
0.780
.The above results were determined by the method of Ostwald (Handbuch
physiko-chemischen Messungen 207 ff.). A thermostat was used and great
care taken to reduce experimental errors and purify the acetylene. The results
are in terms of the Ostwald Solubility Expression, for which see page 227, following.
SOLUBILITY OF ACETYLENE IN AQUEOUS ACETONE SOLUTIONS.
(Kremann and Honel, 1913.)
Vol. Per Cent H2O Cms. CzH.2 dissolved per Liter Sat. Solution at:
in Solvent
(HjO + Acetone).
O
5
10
20
35
5o
75
100
The freezing-point curve for mixture* of acetylene and methyl ether are
given by Baume and German (1911, 1914).
ACETYLENE Biiodide, cis and trans.
Data for the lowering of the freezing-points of mixtures of these two isomers
are given by Chavanne and Vos (1914).
ACONITIC ACID C3H3(COOH)3.
100 grams of formic acid (95% HCOOH) dissolve 2.01 grams C3H3(COOH)S
at 2O.6° C. (Aschan, 1913.)
0°
18°
25°
37
21
15-2
3i
18.2
13-5
26
15-0
io-5
i5
9-5
8.0
8.4
5-5
4-45
5-7
1.23
2.22
1.23
0.98
AOONITINE (Amorphous) C34H47NOU.
SOLUBILITY IN SEVERAL SOLVENTS.
(At 25° U.S.P.; at i8°-22°, Miiller — Apoth.-Ztg. 18. a, '03.)
Solvent.
Water . .
Alcohol .
Ether . .
100 gms.
Cms. CaJItfNOi per
loo Gms. Solvent at:
Solvent
l8°-32°.
0.054
1.44
25°.
0.031
4-54
2.27
Gms. CsilL^NOii pet
100 Gms. Solvent at:
~~^
l8°-22°.
Benzene *7 -%$
Carbon Tetrachloride i . 99
Petroleum Ether . . 0.023 0.028
dissolve 0.0226 gm. aconitine at 22° (Dunstan and Umney, 1892.)
abs. alcohol " 2.7 " " " " (Jiirgens, 1885.)
" ether "- 1.56 "
TrichloroACRYLIC ACID 18
TrichloroACRYLIC ACID CC12:CC1COOH.
SOLUBILITY OF TRICHLOROACRYLIC ACID IN WATER
(Boeseken and Carriere, 1915.)
Gms. CC12:
44
, CC1COOH
t
• per 100 Gms.
Sat. Solution.
O.O
0.0
—0.36
2.0
- 0.6
Eutec. 4.5 :
+13.7
64.1
68.5
17.0
74-5
19.2
m. pt. 80.0
17.0
Eutec. 8 1 . i
20.3
82.8
25.0
84-5
30.0
86.0
40.0
89.5
50.0
92.5
60.0
94-5
70.0
98.5
72.9
IOO.O
Solid Phase.
Ice
Ice+CCl2:
CCl2.CClCOOH.2iH2Q
CC12:CC1COOH+
CC12:CC1COOH.2JH2O
CC12:CC1COOH
Between the concentration 4.5
and 64.1 two liquid layers are
formed. The percentage of
CC12:CC1COOH in each is as
follows:
Gms. CC12:CC1COOH per
t° loo Gms. Sat. Solution.
Lower Layer.
Upper Layer.
10
5-0
20
5-2
64.1
30
6.0
63.8
40
7-5
62.2
50
13-0
59-5
55
18.0
56.0
60
27.0
49.0
62 crit.
t. 38
.0
The original results were plot-
ted on cross-section paper and
the above figures read from the
curves.
ACTINIUM EMANATIONS.
SOLUBILITY IN SEVERAL SOLVENTS.
(Hevesy, 1912.)
A method was elaborated for determining the partition coefficient between a
gas and a liquid phase. The solubility of actinium emanations was then de-
termined in KC1, H2O, H2SO4, CjHsOH, C5HnOH, (CH3)2CO, C6H5CHO, C6H6,
CyHs, petroleum ether and CS2. The solubility increases in the order named.
Close relations are indicated between actinium, thorium and radium.
ADIPIC ACID (Normal) (CH2)4(COOH)2.
100 grams H2O dissolve 1.44 grams adipic acid at 15°.
(Henry — Compt. rend., 99, 1157, '84; Lamouroux — Ibid., 128, 998, '99.)
ADIPINIC ACID (CH2)4(COOH)2.
loo grams of formic acid (95% HCOOH) dissolve 4.04 grams of (CH2)4
(COOH)2 at 18.5°; 100 cc. of the saturated solution contain 4.684 grams of
the acid. (Aschan, 1913.)
AGARIC ACID CioH3oO6.H2O.
IOO grams trichloroethylene dissolve 0.014 gram agaric acid at 15°.
(Wester and Bruins, 1914.)
I9 AIR
AIR
SOLUBILITY IN WATER.
(Winkler — Bcr. 34. 1409. 'ox; see also Peterson and Sondern — Ber. 22, 1439, '89.)
cc.* of atmospheric O and N per liter of:
Dist. HjjO (at 760 mm.). Sea Water (at 760 mm.).
f. B.
o 0.02881
5 -02543
10 .02264
15 .02045
20 .01869
25 .01724
30 .01606
40 .01418
50 .01297
60 .01216
80 .01126
100 .01105
B = " Coefficient of Absorption," i.e.
by the liquid when the pressure of the gas itself without the tension
of the liquid amounts to 760 mm.
Bf = " Solubility," i.e., the amount of gas, reduced to o° and 760
mm., which is absorbed by one volume of the liquid when the barometer
indicates 760 mm. pressure.
* Reduced to o° and 760 mm.
SOLUBILITY OP AIR IN AQUEOUS SULPHURIC ACID AT 18° AND 760 MM.
(Tower — Z. anorg. Ch. 50, 382, '06.)
B'.
Oxygen.
Nitrogen.
Oxygen.
Nitrogen.
0.02864
10.19
18.45
7-77
14.85
.02521
8.91
16.30
6-93
I3-32
.02237
7.87
14.50
6.29
12. 06
.O2OI I
7-04
13.07
5-70
11.05
.Ol826
6-35
II.QI
10.25
.01671
5-75
10.96
...
9.62
•01539
5-24
10.15
•OI3I5
4.48
8.67
.OII4O
3-85
7-55
.00978
3.28
6.50
.OO6OO
1.97
4-03
.00000
o.oo
o.oo
the amount of gas dissolved
Wt. % H2SO4 98 90 80 70
Solubility Coef. 0.0173 0.0069 0.0069 °-°°5S
SOLUBILITY OF AIR IN ALCOHOL, ETC.
(Robinet, 1864.)
60 50
0.0059 0.0076
Vols. Air per 100
Vols. Solvent.
Solvent.
Alcohol (95 . i%) . . 14.1
Petroleum 6.8
Benzene 14.0
Solvent.
Oil of Lavender . .
Oil of Turpentine .
Vols. Air per too
Vols. Solvent.
. . 6.9
. . 24.2
ALANINE (« Aminopropionic Acid) CH3CH(NH2)COOH.
SOLUBILITY IN MIXTURES OP ALCOHOL AND WATER AT 25°.
(Holleman and Antusch, 1894.)
!•%
:ohol.
Gms. per
100 Gms.
Solvent.
Sp. Gr. of
Solutions.
0
16.47
I .0421
5
14-37
I.03II
10
12-43
I .0280
15
10-49
I.OIOI
20
8.48
o 9984
25
7- II
0.9886
31
5-53
o 9761
Vol. %
Alcohol.
Gms. per
100 Gms.
Solvent.
Sp. Gr. of
Solutions.
35
4.91
0.9670
40
3-89
0-9577
5o
2.38
0-9355
60
i-57
0.9102
70
0.85
0.8836
80
o-37
o 8556
See remarks under a Acetnaphthalide, page 13.
100 gms. pyridine dissolve 0.16 gm. a alanine at 20-25°.
.(Dehn, 1917.)
ALANINE 20
SOLUBILITY OF d ALANINE AND OF dl ALANINE IN WATER AT DIFFERENT
TEMPERATURES.
(Pellini and Coppola, 1913.)
Results for:
d Alanine. d — I Alanine. Mixtures d + 1 Alanine.
o
17
3<>
45
ALBUMIN, (Egg).
100 gms. H2O dissolve 100 gms. egg albumin at 20-25°. (Dehn, 1917.)
loo gms. pyridine dissolve o.i gm. egg albumin at 2O°-25°. "
loo gms. aq. 50% pyridine dissolve 6.29 gms. egg albumin at 2O°-25°.
(Dehn, 1917.)
Gms. d Alanine per
100 Gms. IfcO.
12.99
Gms. d — I Alanine pe
100 Gms. H2O.
12.89
r Gms. per 100 Gms. H2O.
d Alanine.
J3-27
/ Alanine".
4-OI
15-17
J4-95
14-5
4.1
17.39
20.55
17.72
21.58
J7.o5
4.99
ALLANTOIN
SOLUBILITY IN WATER.
(Titherly, 1912.)
The author obtained results varying from 0.7 to 0.77 gms. allantoin per 100
gms. H2O at 25°. The variations were considered to be due to slow decompo-
sition of the compound.
ALIZARIN Ci4H602(OH)2.
SOLUBILITY IN WATER AT VARYING TEMPERATURES.
(Hiittig, 1914; Beilstein.)
t°. 2S°.V 100°. 250°.
Grams Alizarin per liter 0.00x3595 0.340 3-OI7
According to Dehn (1917), 100 gms. H2O dissolve 0.04 gm. alizarin at 2o°-25°.
SOLUBILITY OF ALIZARIN IN AQUEOUS SOLUTIONS OF:
Ammonia at 25°. Sodium Hydroxide at 25° (Huttig, 1914.)
Gms. NHs per
Liter.
Gms. Alizarin
per Liter.
Gms. NaOH
per Liter.
Gms. Alizarin
per Liter.
Solid Phase.
0.160
4-025
0.132
0.228
0.427
I .050
I-I59
3.820
C]4H804
Ci4H804 + CnHANa
loo gms. 95% formic acid dissolve o.io gm. alizarin at 20.8°. (Aschan, 1913.)
Alizarin is soluble in all proportions in pyridine and in aqL. 50% pyridine at
20°-25°. (Dehn, 1917.)
ALOIN.
Squires and Caines (1905) found the solubility of aloin in water at room tem-
perature to be 0.83 gm. per 100 cc. and in 90% alcohol, 5.55 gms. per 100 cc.
According to Wester and Bruins (1914) 100 gms. trichloroethylene dissolve
0.013 gm- aloin at 15°.
21 ALUMINIUM BROMIDE
ALUMINIUM BROMIDE AlBr,.
SOLUBILITY IN SEVERAL ORGANIC SOLVENTS.
(Mcnschutkin, 1909-10.)
(Determinations by Synthetic Method.)
In Benzene.
In Para Xylene.
5-7m.pt.
0
4-5
10
3
20
1.8 Eutec.
27.4
10
35-3
20
46.5
30
59
40
70
60
83
80
91.2
90
95-3
96
IOO
Gms. AlBra per
loo Gms. Sat. Solid Phase.
Sol.
QH,
AlBra
Gms. AlBra per
t°. 100 Gms. Sat. Solid Phase.
Sol.
14 m. pt.
0
p QlfcCCHa),
12.5
11.4
r
10.2 Eutec.
25
AlBra+£ QH4(CHi)i
20
35-7
AlBr,
30
47.2
"
40
61.2
M
5°
72.2
M
60
79.6
M
80
90.9
a
90
95-4
M
96
IOO
M
In Toluene.
Gms. AlBrs
per loo Gms. Solid Phase.
Sat. Sol.
•15
O
10
20
30
40
50
70
90
96
16.1
23-7
32.1
42.5
56
68.8
76.5
87.2
95-7
IOO
AlBrs —
In Benzoyl Chloride.
Gms. AlBrs
~
t°.
per loo Gms.
Solid Phase.
Sat. Sol.
— 0.5
m. pt. o
CgHsCOCl
- 2.5
. n-7
1
- 5
Eutec. 22.2
QHsCOCl+AlBra.CgHiCOCl
20
33-7
AlBra-QHsCOCl
40
42.6
"
00
51-6
"
80
60.5
M
90
m. pt. 65.5
M
80
68.9
M
60
71.8
«
30
75-8
"
7
Eutec. 78.8
AlBrl.C6H5COCl+AlBr,
20
80.6
AlBra
50
85.6
«
80
93-2
"
96
IOO
"
Reciprocal solubilities determined by the method of lowering of the freezing-
point (see footnote, page i) are given by Kahlukow and Sachanow (1909) for
mixtures of Aluminium Bromide and each of the following compounds: ani-
line, benzene, benzonitrile, methylbenzoate, p bromaniline, bromobenzene,
methylene bromide, p dibromobenzene, dimethylaniline, diphenylamine, methyl-
aniline, naphthaline, nitrobenzene, p yridine, toluene and p xylene. Similar data
for mixtures of Aluminium Bromide and dimethylpyrone are given by Plot-
nikow (1911).
ALUMINIUM BROMIDE 22
SOLUBILITY OF ALUMINIUM BROMIDE IN SEVERAL ORGANIC SOLVENTS (Con.')
(Determinations by Synthetic Method.)
In Benzophenone.
In Ethylene Bromide^
Gms. AlBrs per
t°. ioo Gm. Sat. Solid Phase.
Gms. AlBrs per
t°. ioo Gm. Sat. Solid Phase.?
Sol.
Sol.
48 m. pt. O (QHfi^CO
10 m. pt. 0 C2H4Br2
45 I2
6 11.5
42 19
2 21.3
38EutCC. 24.7 " +AlBr3.(C6H5)2CO
— 2 EutCC. 29.7 C2H4Br2+AlBn
60 3° • 9 AlBrs. (C«H5)2CO
10 36 . 1 AlBr3
80 36.4
20 42 . I
IOO 42 . 2 "
30 48.7
120 49
40 56
130 53
50 63.7
I42m.pt. 59.5
60 71.5
130 64
70 79.1
ioo 69
80 86.8
70 72.2
90 94.5
50 74
96 ioo
38 EutCC. 75 " +AlBn
50 78 AlBn
•• ".-
80 88
90 93-5
96 ioo
In Nitrobenzene.
In o Chloronitrobenzene.
Gms. AlBrs per
t°. ioo Gm. Sat. Solid Phase.
Gms. AlBrs per
t°. ioo Gm. Sat. Solid Phase.
Sol.
Sol.
5. 5m.pt. o CoHsNOj
32
, 5 m. pt. O o CeHUClNOa
o 18
25
21.8 "
-5 28.8 "
13
. 8 EutCC. 37.5 " +AlBr3.o C6H4ClNOa
-l5EutCC. 42 " +AlBr3.C«HsNO2
30
43 . 1 AlBrs.0 QH^ClNOj
O 44-3 AlBn.QHsNOs
50
50-3
30 49.4
70
57-6
60 56.7
83
,5 m. pt. 62.9
80 63.6
70
67
87m.pt. 68.4
40
73-7
80 71.3
21
EutCC. 77.5 " +AlBrt
60 73.9
40
80 . 6 AlBn
40 76.4
60
84
2oEutCC. 78.9 " +AlBn
80
88.6
40 82 .4 AlBrj
90
93-4
60 85.8
96
IOO
80 89.8
93 96.6
96 ioo
23 ALUMINIUM BROMIDE
SOLUBILITY OF ALUMINIUM BROMIDE IN SEVERAL ORGANIC SOLVENTS (Con.).
(Determinations by Synthetic Method.)
In m Chloronitrobenzene.
In p Chloronitrobenzene.
'
Gms. AlBrs per
t°. 100 Gms. Sat. Solid Phase.
Gms. AlBrs per
t°.. 100 Gms. Sat. Solid Phase.
Sol.
'Sol.
44
.5m.pt. o wC«H4CiN02
83
m. pt. o
£C«H4ClNOi
40
18.9 "
80
9
"
35
. 5 EuteC. 27.8 " +AlBr3.»M C6H4C1NO»
70
24.8
"
50
34.8 AlBrs.»t C6HiClNOj
60
Eutec. 36.6
"+AlBrs.£C6H4ClNOj
70
44-5
80
45-6
AlBrs.£ C6H4C1NO«
90
54-5
100
54-9
"
io3
.5 m. pt. 62.9
MS
m. pt. 62.9
"
90
68.6
100
66.8
"
70
73-4
60
72.4
M
5o
77-3
20
Eutec. 78
" 4-AlBri
40
Eutec. 79.1 " +AlBrj
60
85-3
AlBrs
6o
82.2 AlBrs
80
89.3
H
80
87.t
93
95-4
H
90
92.2
96
100
M
95
95-1
96
100
In o Bromonitrobenzene.
In m Bromonitrobenzene.
Gms. AlBrs per
t°. 100 Gms. Sat. Solid Phase.
Gms. AlBrs per
t°. 100 Gms. Sat. Solid Phase.
Sol.
.Sol.
38
m. pt. o o.
.C,EUBrNOi 54
m. pt. o t
»QH4BrNOj
30
19.7
50
ii. 6
"
21
Eutec. 30
" +AlBrs.o CglMBrNOz 45
.5 Eutec. 19.5
40
37-6
AlBr*> CeH4BrNOa 60
25-5
AlBr3.w QHiBrNOj
60
45-3
80
34-5
"
80
53
no
49-5
•
88
.5m.pt. 56.9
" 122
m. pt. 56.9
it
80
59-7
no
61.6
"
60
64.1
80
69.2
H
40
68.6
60
74.1
"
24
Eutec. 72
" +AlBn 42
Eutec. 78.7
" +AlBn
40
75-5
AlBrs 60
80.3
AlBn
60
79.8
80
84.9
i<
80
86.3
93
93-6
"
93
94-5
;; 96
100
a
96
IOO
ALUMINIUM BROMIDE 24
SOLUBILITY OF ALUMINIUM BROMIDE IN SEVERAL ORGANIC SOLVENTS (Con.}.
(Determinations by Synthetic Method.)
In p Bromonitrobenzene.
In p Nitrotoluene.
Gms. AlBr3 per Gms- AlBrs per
t°. loo Gms. Sat. Solid Phase. t°. 100 Gms. Sat. Solid Phase.
Sol. Sol.
I24.5m.pt. 0 ^.CBHiBrNOa 53.5m.pt. 0 *C«H4CH3NOj
119 10 " 50 10
no
25.2
40
31 .3
"
98 Eutec.
,35-3 "•
{-AlBrs.0 C6H4BrNO2 29 EutCC.
46.1
"+AlBr3.£C4H4CHsNOi
no
39-7 A
[Era.p C6H4BrNOa 50
52.9
AlEr3.p C«H4CHsNOi
130
48.7
80
63
ii
144 m. pt.
56-9
88 m. pt.
66
"
120
65.5
80
68.5
"
90
7o-5
50
74-3
*
60
74.1
27 Eutec.
78.9
" +AlBn
45 Eutec.
76
" +AlBr3 50
83-3
AlBrs
60
79.6
AlBrs 70
87.7
•
80
86.6
8S
92.2
"
93
95-4
93
96.7
ii
96
IOO
96
IOO
"
In m Nitrotoluene.
In o Nitrotoluene.
i —
16
12
Gms. AlBrs
t°. per loo Gms. Solid Phase.
Sat. Sol.
m. pt. 0 m CjHiCHsNOa
14-5 "
Gms. AlBr3
t°. per loo Gms. Solid Phase.
Sat. Sol.
— 8 . 5 m. pt. 0 o C6H4CH3N02
— II EuteC. 8.7 !'-J- AlBrs. 2oC«H4CHsNO2
8
21.8 "
10
12.8-
MBr3.20C«H4CaNOa
• I
EuteC. 32 "+AlBrs.»» QEUCHsNOz
30
24.8
"
20
38.5 AlBrs-m CeHiCHsNOj
40
38
"
40
46.6
42
.5 Eutec. 47.7
"+ AlBrs.aoCjHjCHsNO!
80
59-7
60
54-3
AlBrs.o C6H4CHsNOj
90
63.3
75
59-5
"
96
m. pt. 66
90
m. pt. 66
"
90
68.8
70
72
"
60
73-8
40
76.1
"
27
EuteC. 78.9 " +AlBr3
19
Eutec. 79.1
" +AlBa
40
82 AlBr,
40
82.5
AlBrs
70
89
70
87.5
"
90
95-3
90
93-8
"
96
IOO
96
IOO
"
ALUMINIUM CHLORIDE
ALUMINIUM CHLORIDE A1C13.6H2O.
SOLUBILITY IN WATER.
(Gerlach — Z. anal. Ch. 8, 250, '69.)
ioo gms. saturated solution contain 41.13 gms. A1C13 at 15°, Sp. Gr. of solu
tion = 1.354.
SOLUBILITY OF ALUMINIUM CHLORIDE IN SEVERAL ORGANIC SOLVENTS.
(Menschutkin, 1909.)
(Determinations by Synthetic Method.)
In Nitrobenzene. In o Chloronitrobenzene.
Gms. A1CL,
t°. per ioo Gms. Solid Phase.
Gms. A1CU
t°. per ioo Gms. Solid Phase.
Sat.
Sol
Sat ~
.Sol.
5
•5
m. pt.
0
CgHsNOj
32
.5 m. pt. o
o C,H4C1N02
2
Eutec.
10
•3
" +A1CU.2C6H5N02
27
10
.2
"
15
18
A1C13.2C.H5NO2
21
16
.1
"
25
-5
Eutec. 30 . 5
" +A1C13.C6H5NO2
15
Eutec. 20
•3
" +A1C13.0C.H4C1N02
45
34
.2
AlCls.CelfcNOi
35
25
•5
AlCls.o C6H4ClNOj
65
39
•5
"
55
31
•5
"
85
48
"
75
38
•7
tt
90
m
.pt.
52
"
89
m. pt. 45
•9
"
82
55
.6
"
80
51
tt
72
58
"
69
Eutec. 54
•4
" +A1C1.
52
Eutec.
61
.6
"+A1C1,
no
. 57
•5
A1CU
90
64
A1C1*
150
65
•4
"
130
67
•7
"
175
74
.6
"
160
72
•4
"
194
IOO
"
180
80
.1
"
194
IOO
In m Chloronitrobenzene.
In p Chloronitrobenzene.
t°.
Gms. A1CU
per ioo Gms.
Sat. Sol.
Solid Phase.
44 . 5 m. pt. O m C8H4ClNOa
44 10.7 "
36 Eutec. 16.6 "+Aici3.w c6H4CiN02
50 21
70 28.3
90 36.8
104 m. pt.
90
81 Eutec.
120
140
160
45-9
52-4
55-6
60
64.1
70.2
" +A1CU
A1CU
Gms. A1CU
t°. per ioo Gms. Solid Phase.
Sat. Sol.
83
.5 m. pt. o
p C6H4ClNOa
78
7.1
"
73
12.8
"
68
Eutec. 17.1
" +MC\3.p C8H4C1NO,
80
22.2
MOa.p C4H4C1NO»
IOO
31-4
"
120
41.8
"
126
m. pt. 45.9
•
no
53-2
"
94
Eutec. 58.1
"+ AlCli
125
60.5
AlCli
155
66.9
s. - "
180
77-7
M
190
88.2
"
104
IOO
"
The solubility of aluminium chloride in anhydrous hydrazine is stated by
Welsh and Broderson (1915) to be i.o gm. in ioo cc. at room temperature.
ALUMINIUM CHLORIDE 26
SOLUBILITY IN SEVERAL ORGANIC SOLVENTS (Con.).
(Determinations by Synthetic Method.)
In o Bromonitrobenzene.
In m Bromonitrobenzene.
Gms. AlCb
t°. per 100 Gms. Solid Phase.
Gms. AlCb
t°. per 100 Gms. Solid Phase.
Sat. Sol.
Sat. Sol.
38.5
0 o QlfcBrNO,
54
•7 o
m C6H4BrNOa
32
7-5 "f
51
6.5
"
26
47
Eutec. 11.9
"+ AlCU.ro C6H4BrNOi
20 Eutec.
17.5 " +A1C13.0 C6H4BrNOa
60
16
AlCb.ro C6H4BrNO»
40
21.7 AlCb.o C»H4BrNO»
80
22.9
"
60
26.4
100
30.7
"
80
31.7 "
no
35-9
«
97 m. pt.
38
116
m. pt. 39.8
M
100
39.8
H3
42.3
««
90
44.6
107
44-5
•
80 Eutec.
46.5 " +A1CU
97
Eutec. 47.4
"+A1CU
no
50.1 Aid,
120
5i-5
A1CU
130
54-1
140
56.5
"
150
60.2
160
64-5
"
170
70
180
77-4
«
180
77-4
190
88.8
M
197
100
U
In p Bromonitrobenzene.
In o Nitrotoluene.
^
Gms. AlCb
Gms. AlCb
t°. per zoo Gms. Solid Phase.
t°. per 100 Gms. Solid Phase.
Sat. Sol.
Sat. Sol.
124
, 5 m. pt. 0 P QI&BrNOa
— 8.5 HI. pt. O o C6H4CH3N02
117
7-4 "
— 9.3 EuteC. I "+AlCb.2o C,H4CTfcNOi
III
12.8 "
0 1-5 AlCb.20 CeHiCHsNOi
105
17.7 "
20 4
99
EuteC. 22.2 "+AlCb.£ CVEfcBrNOa
40 II
120
28 . 4 MC\a.p CjHiBrNOj
<< EuteC. 31 " +AlCb.o C«H4CHjNOj
\s \s \s
I4O
36.4
85 41.8 AlCb.o C6H4CH3NOj
145
m. pt. 39.8
95. 5m. pt.49.3
140
44-5
70 56.8
120
51-2
45 Eutec. 61.5 "+AICI,
"3
Eutec. 52.8 "+AICU
95 64.5 Aicb
130
55.9 AlCb
145 73-7
150.
61.3
180 86.2
180
77-4
185 89.5
190
88.8
194 100
194
100. 0
One liter sat. solution of A1C13 in CC14 contains 0.74 gm. at 4°, 0.22 gm. at 14°,
0.15 gm. at 20° and 0.06 gm. at 34°.
One liter sat. solution of A1C13 in CHC13 contains 0.65 gm. at — 15°, i.o gm at
o° and 0.72 gm. at 25°. (Lloyd, 1918.)
ALUMINIUM CHLORIDE
SOLUBILITY IN SEVERAL ORGANIC SOLVENTS (Con.).
(Determinations by Synthetic Method.)
In m Nitrotoluene.
In p Nitrotoluene.
'
Gms. AlCla
Gms. A1CU
t°. per 100 Gms. Solid Phase.
t°. per 100 Gms. Solid Phase.
Sat. Sol.
Sat. Sol.
i6
m. pt. 0 m CeHiCHsNCb
52
. 5 m. pt. 0 P CaHUCHaNOj
13
EuteC. 7.8 "+AlCl3.2wC6H4CH3NOa
47
9.2 «
27
13 .4 A1C13.2W CfrfoCHsNOz
42
15 "
35
EuteC. 24.5 "+AlCl3.«tC6H4CH3NOa
37
EuteC. 19 "+AlCU.0CeH4CHsNO,
65
34 AlCls.w CeEUCHsNOa
55
29 . 1 AlCla.* C«H4CH,NOi
90
44.2
80
34-8
95
46.7
95
41.3
99
.Sm.pt. 49. 3
109
m. pt. 49.3
70
56.8
100
53-4
45
Eutec. 61.5 "+Aici3
60
61.7
95
64 . S AlCla
45
Eutec. 64 " +Aicii
120
68.2
105
69 . 5 AlCli
130
70.2
165
80
190
94-3
194
IOO.O
In Benzophenone.
In Benzoyl Chloride.
f
Gms. AlCls
\
Gms. AlCls
t°. per loo Gms. Solid Phase.
t°. per 100 Gms. Solid Phase.
Sat. Sol.
Sat. Sol.
48
m. pt. 0 (C8H5)2CO
— o.
5 m. pt. 0 CeHsCOCl
44
8-5 -
4
7.9 "
39
. 5 Eutec. 15.4 " +Aici3(c,H5)2CO
-7-
S Eutec. 12.7 " +Aici3.c,H6coci
60
19.3 AlCl3.(C6H5)*CO
o
14 . 1 AlCU-QHsCOCl
90
26 . s
20
18.8
120
37
40
25
130
m. pt. 42.3
60
33
110
48.8
80
42.2
80
53-5
93m.pt. 48.7
60
Eutec. 56 . i " +AICU
80
52.9
100
58 AlCli
60
57.2
140
63
40
61
160
68.6
180
78.5
190
89.1
•
192
93
104
100
ALUMINIUM FLUORIDE A1F3.
Fusion-point data (Solubility, see footnote, page i) are given by Pushin and
Baskov (1913) for the following mixtures:
A1F3 + NaF, A1F3 + KF, A1F3 + LiF, A1F3 + CsF, A1F3 + RbF.
Similar data for mixtures of A1F3 + NaF are given by Fedotieff and Illjinsky
(1913).
ALUMINIUM HYDROXIDE
28
ALUMINIUM HYDROXIDE A1(OH)3.
SOLUBILITY OF MOIST FRESHLY PRECIPITATED ALUMINIUM HYDROXIDE IN
AQUEOUS SOLUTIONS OF ALUMINIUM SULPHATE.
(Kremann and Hiittinger, 1908.)
Results at 40°.
Results at 20°.
Gms. per zoo Gms. H2O.
'A12(SO4)3.
Al(OH)a.
2-37
0.15
A12O3.SO3.9H2O
5
0.30
tt
7
0.65
tt
9.1
1.30
Transition Point
10
1.23
Al2O32SO3.i2H2O
15
1.04
"
20
1.40
tt
25
2.40
11
3°
3-70
tt
31.6
4.20
Transition Point
33
2-75
Al2O3.3S03.i6H2O
34-73
0.92
tt
Gms. per 100 Gms. HbO.
Al(OH)r
Solid Phase.
5.22
. . .*
Transition Point
8.85
1.82
Al2O3.2SO3i2H20
10
1.65
tt
15
1.40
ft
20
2-15
"
25
3.80
"
28.5
5.80
Transition Point
30
4-35
Al203.3SO3.i6H2O
35
i. 60
tt
49
0.60
ft
Results at 60°. f
Gms. per 100 Gms. HzO.
* The figures given are not sufficient to deter-
mine this transition point accurately.
t The author's figures for 60° are reproduced
without change as they are not sufficient to deter-
mine transition points.
A12(SO4)3.
3-24
8.83
12.67
24.07
31-55
42.38
49 -85
A1(OH)3
2-53
I.8S
4.89
6.02
1.42
Solid Phase.
A12O3.SO3.9H2O
Al203.2S03.i2H2O
Al2O3.3S03.i6H2O
SOLUBILITY OF ALUMINIUM HYDROXIDE IN AQUEOUS SODIUM HYDROXIDE
SOLUTIONS. (Haber and van Oordt, 1904.)
The mixtures were agitated for 24 hours- So-called acetic acid soluble tonerde
(E. Merck) was used for the experiments. Temp. 2O°-23°.
Normality of Aq. NaOH. Gms. AUOa per Liter.
0.49 9.27
0.99 13.90
2.OO 14.40
SOLUBILITY OF ALUMINIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF SODIUM
HYDROXIDE. (Herz, 1911; Slade, 1911 and 1912.)
The experiments show that the ratio of Na to Al in the solution varies con-
siderably depending upon whether the used Al hydroxide was precipitated hot
or cold, also upon the length of time it was dried and upon the nature of the
drying agent. Herz found a nearly constant ratio of 3 Na to I Al in solution.
Slade gives ratios of approximately 2.5 : 1 in normal NaOH at 25° for cold pre-
cipitated hydroxide dried over HgSCX and 9.0 : I for hot precipitated Al hydroxide
dried over PzO^ Drying in thin layers also increased this ratio but to a some-
what less extent. Slade reports the solubility of A1(OH)3 in a 0.6414 normal
NaOH solution to be 1.34 gm. per 100 cc. at room temperature.
ALUMINIUM OXIDE A12O3.
m Fusion-point lowering data for mixtures of aluminium oxide and cryolite are
given by Lorenz, Jabs and Eitei (1913). The results show one eutectic at ap-
proximately 940°. The eutectic mixture contains 19.8% A12O3.
Results for aluminium oxide and magnesium oxide are given by 'Rankin and
Merwin (1916).
29 ALUMINIUM SULFATE
ALUMINIUM SULFATE Al2(SO4)3.i8H2O.
SOLUBILITY IN WATER.
(Poggiale, 1843; Kremann and HUttinger, 1908.)
Mid Phase. t°. ^G^^tToL SoM Phase.
AU(SO4),.i8HiO
—
I
.02
8
.09 Ice
20
26
•7
—
I
•43
10
•7
30
28
.8
—
2
.04
14
•3
40
31
•4
—
2
-65
17
•5
50
34
•3
—
2
•85
19
.2
60
37
.2
—
4
Eutec.
23
. I Ice + Al2(SO4)3.i8H2O
70
39
.8
o
23
. 8 Al2(SO4)3.l8H2O
80
42
.2
-f-
7
•73
24
.8
90
44
•7
10
25
.1
IOO
47
.1
SOLUBILITY OF ALUMINIUM SULFATE IN AQUEOUS SOLUTIONS OF FERRIC
SULFATE AT 25° AND VICE VERSA. (Wirth and Bakke, 1914.)
Gms. per 100 Gms. Sat. Sol. . Gms. per 100 Gms. Sat. Sol.
•AWSO.).. ' Fe,(SO.),. SohdPhaSe- 'AMSO.),. ' Fe^SO.)..' S<"'d "—
27.82 O . Ak(SO4)3.i8H2O 10.03 32-42 Fe2(SO4)3-9H2O
26.01 6.064 " 8.819 34-02
24.21 9.819 " 6.626 35.82
21.64 13-02 " 5-200 38.83
15.22 23.28 2.342 42.44
10.46 31.90 " +Fe2(SO4)3.9H2O ... 44-97
EQUILIBRIUM BETWEEN ALUMINIUM SULFATE, LITHIUM SULFATE, AND WATER
AT 30°. (Schreinemaker and De Waal, 1906.)
Composition in Weight per cent:
Solid
Phase.
Of Solution.
Of Residue.
% Li2S04.
% A12(S04)3.
% Li2SO4.
% A12(SO4)3.
25.1
0
21-93
5-34
16.10
14-89
63.70
4-02
13.63
20.76
14.72
3I-I7
13.24
21 .71
61 .24
7.22
"•73
22.08
6.92
33-54
6-75
24-34
3-77
37.06
3-44
26.12
o.o
28.0
. . .
{ Al2(So!)3.i8H20
Li2S04.4H20
Al2(S04)3.i8H20
SOLUBILITY OF ALUMINIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 25°. (Wirth, 1912.)
Gms. per IOo Gms. Sat. Sol - Gms. per 100 Gms. Sat Sol.
'Al2(S04)s. H2S04. " ' Al2(S04)3. H2S04.
27.82 O AU(SO4)s.i8H2O 4.8 40 Ali(SO4)3.i8HzO
29.21 5.13 1.5 5°
26.2 10 i 60
19.5 20 2.3 70
11. 6 30 4 75
A curve was plotted from the published results and the above figures read
from the curve.
loo gms. glycol dissolve 16.82 gms. A12(SO4)3. We Coninck, 1905-)
ALUMINIUM SULFIDE A12S3.
Fusion-point data for mixtures of Al2Sa + Ag2S are given by Cambi (1912).
ALUMS
ALUMS.
SOLUBILITY OP AMMONIUM ALUM AND OP POTASSIUM ALUM
IN WATER.
(Mulder; Poggiale — Ann. chim. phys. [3] 8, 467, '43; Locke — Am.Ch. J.26, 174, '01; Marino —
Gazz. chim. ital. 35, II, 351, '05; Berkeley — Trans. Roy. Soc. 203 A, 214, '04.)
O
5
10
15
20
25
30
40
50
60
70
80
90
92.
95
Ammonium Alum.
Potassium Alum.
Gms. (NH4)2 Gms.
Al2(S04)4 A12(S04J424H20
per 100 g.
H20.
G.M.(NH4)2
A12(S04)4
per 100 g.
H20.
Gms. K2
A12(S04)4
per 100 g.
H20.
Gms. K2 G. M. K2
A12(S04)424H20 A12(S04)4
per
2.10
3-90
O.OO44
3-o
5-65
0.0058
3-5°
6.91
O.OO74
3-5
6.62
0.0068
4-99
9-52
O.OIO5
4-0
7.60
0.0077
6.25
12.66
0.0132
5-o
9-59
0.0097
7-74
15.13
0.0163
5-9
ii .40
O.OII4
9.19
19.19
O.OI94
7-23
14.14
0.0140
10.94
22 .OI
0.0231
8-39
16.58
0.0162
14.88
30.92
0.0314
11.70
23-83
0.0227
20.10
44-10
O.O424
17.00
36.40
0.0329
26 . 70
66.65
0.0569
24-75
57-35
0.0479
40.0
110.5
0-0774
71.0
321-3
0-1374
...
...
109.0
2275.0
0.2IIO
119.0
GO.
0-2313
109.7
CO
0.2312
NOTE. — The potassium alum figures in the preceding table were
taken from a curve plotted from the closely agreeing determinations of
Mulder, Locke, Berkeley, and Marino. For the higher temperatures
(above 60°), however, the results of Marino are lower than those of
the other investigators, and are omitted from the average curve.
Locke called attention in his paper to the fact that Poggiale's results
upon ammonium and potassium alum had evidently become inter-
changed through some mistake. This explanation is entirely sub-
stantiated, not only by Locke's determinations, but also by those of
Mulder and Berkeley. The ammonium alum figures given above were
therefore read from Poggiale's potassium alum curve, with which
Locke's determination of the solubility of ammonium alum at 25° is in
entire harmony.
SOLUBILITY OF AMMONIUM ALUM IN PRESENCE OF AMMONIUM SULFATE AND IN
PRESENCE OF ALUMINIUM SULFATE IN
Mixture Used.
(Rudorff — Ber. 18, 1160, '85.)
100 Gms. Saturated Solution Contain:
Saturated Ammonium Alum at 18.5° . . . .
20 cc. above sol. + 6 gms. cryst. A12(SO4)3 .
20 cc. above sol. + 4 gms. cryst. (NH4)2SO4.
Grams (NILJjjSCU + Grams Al^SO*)*
. . 1.42 3.69
0-45
20. 8l
16.09
0.29
ALUMS
SOLUBILITY OF MIXTURES OF POTASSIUM ALUM AND ALUMINIUM SULFATE
AND OF POTASSIUM ALUM AND POTASSIUM SULFATE IN WATER.
t°.
o
20
35
65
77
o
5-
10
*5
30
40
60
3o
(Marino — Gazz. chim. ital. 35, II, 351, '05.)
Gms. per 1000 Gms.
Al2(S04)3.i8H20.
K2S04.
243-73
23-45
824-25
30.85
911 .02
35-29
1243.21
59-55
1598.00
ii9-43
l872.II
183.80
5-06
75 -83
8.66
75 •I8
16.07
85.78
18.52
96.50
20.56
109.30
39.60
147-8
73-88
163.1
126.0
195-4
249.7
238.8
529.0
323-7
1044.0
5*7-27
Gm. Mols. per ti OOP Mols. H2O.
Al2(S04)3.i8H20. K2S04."
6.1
Solid
Phase.
24.1
33-5
o.i
O.2
0-4
o-5
o-55
i .o
1.9
3-4
6.7
14.2
28.1
2-3
3-6
6.1
12.6
18.9
7.8
7-7
8.8
9-9
II .2
15.2
16.8
20. i
24.6
32.6
53-4
K2A12(SO4)2.24H2O
+ A12(S04),
K2A12(S04)2.24H20
+ K2S04
SOLUBILITY OF MIXTURES OF POTASSIUM ALUM AND OF THALLIUM
ALUM IN WATER AT 25°.
(Fock — Z. Kryst. Min. 28, 397, '97.)
K,A12(S04)4.24H,0 ; T12A13(SO4)4.24H2O.
Composition of Solution.
A . ._
Solid Phase
Mol. % of
Potassium
Alum.
KAl(S04)2j>er Liter.
T1A1(SO4)2 per Liter.
Grams. Mg. Mols.
Mol. % Sp. Gr. of
KA1(S04)2. Solutions.
Grams.
Mg. Mols.
69.90
270.5
o.oo
o-oo
ioo i -0591
IOO-O
74-56
288.2
0.48
1-13
99.61 I. 0601
99-32
67.90
262.8
1.72
4-07
98.48 1.0598
96.84
65-30
252.7
4-52
10.67
95-95
.0603
90.84
64 95
25I-4
9.60
22.67
91 .73
.0605
82.94
53-23
205-9
18.44
43.56
82.54
.0609
68.24
45-32
175-4
24.60
58.10
75-12
.0609
58.23
38.02
147.2
32-48
76.75
65-73
.0611
46.72
34-54
133-6
35-59
84.10
61.36
.0611
44.23
28-35
109-7
42.99
101.60
5*-93
.0623
32.07
10.94
42.4
66.12
156.2
21.34 1-0654
7-94
o.oo
O-O
75-46
178-3
o.oo 1.0674
o.oo
Data for the influence of pressure on the solubility of potassium alum in
water at o° are given by Stackelberg, 1896.
Data for the solubility of Rubidium Alums are given on p. 582.
ALUMS
SOLUBILITY OF SODIUM ALUM IN WATER.
(Smith, 1909.)
Gms. Na2Al2(SO4)4 per 100 Cms.
Cms. Na2Al2(S04)4.24H20 per 100 Gms
Sat. Sol.
26.9
27.9
Water.
36.7
38.7
29
40.9
3O.I
31-4
43-i
45-8
'
Sat. Sol.
Water.
IO
50.8
I03.I
15
52.7
III.3
20
54-8
121 .4
25
56-9
I3I.8
30
59-4
146.3
10
15
20
25
30
Above 30°, sodium alum is decomposed in contact with its saturated solution.
The exact temperature of transition has not been determined.
Single determinations differing from the above are given by Tilden (1884)
and by Auge (1890).
SOLUBILITY OF CAESIUM ALUM, RUBIDIUM ALUM, AND OP THALLIUM
ALUM IN WATER.
(Setterburg~Liebig's Annalen, 211, 104, '82; Locke — Am. Ch. J. 26, 183, '01; Berkeley — Trans.
Roy. Soc. 203 A, 215, '04.)
Thallium Alum.
Gms. per 100 Gms. H2O.
t°.
Caesium Alum.
Gms. per 100 Gms. H2O.
Al2Cs2(S04)4.
Al2Cs2(S04)4
.24H2O.
o
0.21
o-34
5
0.25
0.40
10
0.30
0.49
20
0.40
0.65
25
0.50
0.81
30
O.6o
0.97
40
0.85
1.38
50
1.30
2. II
60
2.0O
3-27
70
3-20
5-27
80
5-40
9-01
90
10.50
i8.ii
100
22.70
42-54
Rubidium Alum.
Gms. per 100 Gms. H2O.
Al2Rb2(S04)4. Al2^f(2o°*)4
0-72
I. 21
0.86
1.48
1.05
1.81
1.50
2-59
i. 80
3.12
2.20
3-82
3-25
5-69
8.50
7.40
13-36
12.40
23-25
21. 60
43-25
A12T12(S04)4.
A12T12(SO<
3-15
'4.84
3.8o
5-86
4.60
7.12
6.40
10.00
7.60
11 -95
9-38
14.89
14.40
23-57
22.50
38-41
35.36
65.19
NOTE. — Curves were plotted from the closely agreeing determina-
tions recorded by the above named investigators and the table con-
structed from the curves.
Recent determinations of the solubility of caesium alum in water, by Hart
and Huselton (1914), agree well with the data in the above table. For addi-
tional caesium alums see page 180.
SOLUBILITY OF Ammonium Chromium Alum IN WATER.
(Koppel, 1906.)
It was shown that, due to the transition between the violet and green forms
of the compound, the saturation point is reached very slowly, especially at the
higher temperatures. From the determinations at o° it was found that equi-
librium is reached in 2\ hours. If this saturation time is taken for the other
temperatures, the results are considered to show the solubility of the violet
form alone. The final saturation represents the attainment of an equilibrium
between the violet and green forms.
Results for the Violet Form.
Results for Final Equilibrium.
~-
Time of
Gms.
r
Time of
Gms.
t°.
Saturation,
(NH4) Cr (S04)2
t°.
Saturation,
(NH4)Cr(S04)2
Hrs.
per 100 Gms. Sol.
Hrs.
per 100 Gms. Sol.
0
2-5
3-8
0
2-5
3-8
30
2-5
10.6
30
300
I5.7-I6
40
2-5
15-5
40
250
24.5-24.8
33
AMMONIA
AMMONIA NH3.
SOLUBILITY OP AMMONIA IN WATER.
(Roscoe and Dittmar — Liebig's Annalen, 112, 334, '59; Raoult — Ann. chim. [5] i, a6a, '74; Mallet —
Am. Ch. J. 19, 807, '97.)
-40
-30
— 20
— 10
O
5
10
15
At 760 mm.
Pressure.
G.NH3
Vol. NH3
per 100 g.
H2O.
per i g.
1l20.
294.6
278.1
...
176.8
III-5
87-5
1299
77-5
1019
67.9
910
60.0
802
20
25
30
35
40
45
5o
56
At 760 mm.
Pressure.
G.NH3
per 100 g.
H20.
Vol. Nils
per i g.
52.6
46.0
40-3
710
635
595 (28°)
35-5
30-7
27.0
...
22.9
...
SOLUBILITY OF AMMONIA IN WATER DETERMINED BY METHOD OF LOWERING OF
FREEZING-POINT.
(Rupert, 1910.)
j.o vjins,
INX13 PC
f Solid Phase.
0
0
Ice
— 2
2
"
- 4.6
4
"
- 7.6
6
"
— 10.6
8
*
- 13-9
10
it
- 17.6
12
. tt
- 21.4
14
tt
- 25.8
16
ft
18
ft
- 37
20
tt
- 43-6
22
«
- 50-7
24
ft
- 60.3
26
it
- 72.2
28
"
-87.2
30
tt
-102.3
32
tt
— 116.7
34
"
— 120 Eutec.
34-5
Ice + NHjH2O
-103.8
36
NHjHjO
- 92-9
38
"
- 86.7
40
"
- 83.5
42
ft
- 81.4
44
tt
- 80
46
"
- 79-3
48.7
it
- 79-4
50
"
t°
Cms. NHa per
100 Gms. Sol.
Solid Phase.
-80.6
52
NHsHjO
-82.8
54
M
-85.8
56
"
-87
Eutec. 56 . 5 N
Hs.H2O+2NH3.Hj
-84.8
58
aNHaHzO
-82.2
60
"
-80.4
62
«
-79.2
64
a
-79.8
m. pt. 66
tt
-79.2
68
"
-80.3
70
"
-82.1
72
it
-84.5
74
it
-87.4
76
it
-90.4
78
it
-93-6
80
it
-94
Eutec. 80.3
2NH3.HjO-f-NHi
-91.7
82
NHi
-89.4
84
"
-87.4
86
"
-85.6
88
it
— 84.1
90
"
-82.7
92
M
-81.5
94
M
-80.3
96
"
-79.1
98
It
-78
100
*
More recent data on the above system, by Smits and Postma (1914) agree
quite closely with the above except in the region of the eutectic Ice + NH3H2O.
These authors report a temperature of —100.3 instead of —120 for this point.
Additional determinations are also given by Baume and Tykociner (1914). Older
data for the ice curve are given by Guthrie (1884) and Pickering (1893).
' o1
10°.
20
30°.
40°.
50°.
60°.
*
4
•5
9
17
•5
31
5
55
125
149.
5
13
18
32
•5
56.
•5
91
146
234
20
27
47
•5
83
134.
5
210
327
*
27
•5
40
70
IX5
183-
5
28l
425
35
54
93
153
•5
241.5 363.5
539-
5
45
69
118
193,
•5
303-
5
455
666
57
•5
89
151
245
377.
5
564
816.
5
75
"5
191
305
5
465-
5
688.5
985
93
144
237
393
569.
5
834.5
1191
117
180.5
291
455
5
690
1005
1432
144
•5
226.5
360
561.
5
830.
5
1195
...
181
280
440
680
1007
...
• • •
222
346
537
8i7
1189.
5
AMMONIA 34
VAPOR PRESSURE OF AQUEOUS AMMONIA SOLUTIONS.
(Perman, 1903.)
G s NHs oer Vapor Pressure in mm. of Mercury at:
100 Cms. Sol.
O
2.5
5
7-5
10
12.5
15
I7-S
20
22.5
25
27-5
30
The apparatus (Perman, 1901) used for the above determinations, consisted
of a pipet provided with a stop-cock at its upper end and connected with a
Hg leveling tube at its lower end. For maintaining constant temperatures the
vessel was surrounded by a glass jacket into which water or vapors of liquids
boiling at various temperatures could be introduced. The aqueous ammonia
solution was drawn in above the Hg and boiled to expel air. A portion of it
was withdrawn for analysis through the stop-cock at the top, by elevating the
level of Hg. The vapor pressures of the analyzed mixture at various constant
temperatures were then read with the aid of an adjacent millimeter scale. Curves
were plotted from the results and readings for regular intervals of concentration
and temperature made.
By means of a modification of the above apparatus the author was also able
to estimate the partial pressure of the ammonia and of the water of each mix-
ture. Tables for these values are given. Data have also been calculated for
the latent heat of evaporation of aqueous ammonia solutions.
INFLUENCE OF SALTS AND OTHER COMPOUNDS ON THE VAPOR PRESSURE OF
AQUEOUS AMMONIA SOLUTIONS.
(E. G. Perman, J. Chem. Soc. (Lond.), 81, 480, 1902.)
Vapor pressure determinations were made as above described on aqueous
solutions of the following compositions — (a) 10.43% Urea -+- 16.36% NHs,
(b) 5-29% Urea + 17.22% NH3, (c) 4.56% Mannitol + 12.27% NH3, (d) 3.05%
K2S04 + 749% NH3, («) 5.27% NH4Cl + 16.85% NH3, (/) 10.26% NH4C1
+ 12.9% NH3f (g) 2.68% CuS04 + 14-65% NH3, (h) 3.94% CuSO4 + 6.54%
NH3.
The author's data were plotted on cross section paper and the following values
read from the curves.
t°. Vapor Presure of Each Solution in mm. of Mercury.
(a)
(b)
to
(d)
(e)
(/)
tt
(*)
20
204
200
120
. . .
193
130
155
. . .
30
325
325
198
. . .
302
220
235
87
40
485
500
3H
200
471
345
365
145
50
715
727
465
304
695
522
545
223
60
1050
1060
705
453
975
770
344
In an earlier paper Perman (1901) gives data similar to the above for the
vapor pressure of ammonia in aqueous solutions of sodium sulfate.
35 AMMONIA
MUTUAL SOLUBILITY OP AQUEOUS AMMONIA AND POTASSIUM CARBON-
ATE SOLUTIONS.
(Newth — J. Chem. Soc. 77. 776, 1900.)
The solutions used were: Potassium Carbonate saturated at 15°
(contained 57.2 grams K2CO3 per 100 cc.). Aqueous Ammonia of
0.885 Sp. Gr. (contained about 33 per cent ammonia). The determina-
tions were made by adding successive small quantities of one of the
solutions to a measured volume of the other, and observing the point
at which opalescence appeared.
Saturated K2CO3 in Aq. Ammonia. Aq. Ammonia in Saturated
t*. cc. KaCOa per %K2COa Solution cc. Ammonia %K2COa Solution
100 cc. Ammonia, in Mixture. in 100 cc. K2COa. in Mixture.
i 2.0 2.0 37.5 72.7
6 3.0 3.0 47-5 67-6
ii 5-0 4-7 52-5 65-o
16 6.5 6.1 % 60.0 63.0
21 8.5 8.0 77-5 56-3
26 10.5 9.5 105.0 49-0
31 12.5 ii. i 152.5 39.0
38 20.0 16.6 i9S-o 33 -°
39 21 .o 17.0 220- o 31-0
42 25.0 20.0 250.0 28.5
43 35.0 26.0 285.0 26.5
Above 43° the solutions are completely miscible. If 10 per cent of
water is added to each solution the temperature of complete miscibility
is lowered to 25°. The mutual solubilities are:
Per cent K2CO3 Solution in;
t°. Ammonia K2CO3 Sol.
Layer. Layer.
o 8 62
10 ii 52
20 15 38
25 (crit. pt.) 25
With the addition of 12.9 per cent of water to each solution the
temperature of complete miscibility (crit. pt.) is lowered to 10°. With
the addition of 18.1 per cent water this temperature becomes o°.
SOLUBILITY OF AMMONIA IN AQUEOUS SALT SOLUTIONS.
(Raoult.)
In Calcium Nitrate Solutions In Potassium Hydroxide Solutions
Gms. NHa per too Gms. NHa per 100
Cms. Solvent in: Gms. Solvent in:
t*. 28.38% In 59.03% n-25%
Ca(N03)2. CMJ88S KOH
o 96.25 104.5 72-o 49-5
8 78.50 84.75 57-o 37-5
16 65.00 70.5 46-0 28.5
24 373 21.8
The freezing-point curve for mixtures of ammonia and ammonium thiocyanate
is given by Bradley and Alexander (1912).
AMMONIA 36
SOLUBILITY OF AMMONIA IN AQUEOUS SALT SOLUTIONS AT 25°.
(Abegg and Riesenfeld, 1902.)
The determinations were made by the dynamic method of vapor pressure
measurement previously used by Doyer (1890), Konowalow (1898), Gahl (1900),
and Gaus (1900). It consists in passing an indifferent gas through an aqueous
ammonia solution of known concentration and calculating the vapor pressure
from the volume of indifferent gas required to remove a definite amount of
ammonia from solution. The indifferent gas (H + O) was generated by an
electric current and its volume measured by means of a voltmeter. The accom-
panying ammonia was removed by passing through o.oi n. HC1 and estimated
by means of electrolytic conductivity. The molecular vapor pressure was
obtained by dividing the absolute vapor pressure, calculated from above meas-
urements, by the concentration (normality) of the ammonia. For i n. am-
monia in water at 25° the molecular vapor pressure was 13.45 mm- Hg; for
0.5 n. solution it was 13.27 mm. Hg.
Since it has been shown by much experimental evidence, that Henry's Law of
the proportionality of the concentration in the liquid and vapor phase applies
very closely in the present case, see also Gaus (1900), it follows that the am-
monia pressure relation of two solutions of equal ammonia content is recipro-
cally proportional to the solubility relation of the ammonia in them. Hence,
to calculate the solubility from the vapor pressures, it is only necessary to divide
the value for the molecular vapor pressure in H2O by that for the salt solution.
Thus the solubility of NH3 in HzO becomes unity. All determinations were
made with i n. aqueous ammonia in salt solution of 0.5, i and 1.5 normality.
The figures therefore show mols. NH3 per liter of the particular salt solution at
25°. In a later paper by Riesenfeld (1903), additional determinations are given
for 35°.
Salt
Mols. NH3
per
Liter S
altS
iol. of:
Salt
Mols. NH3 per Liter Salt Sol. of:
Solution.
0.5 n.
i n.
i
•5n.
Solution.
0.5 n.
i n.
i-S n.
KC1
0.930
0
.866
O
.809
KCN
O
.926
o
.858
O.8O2
KBr
0.950
O
.904
O
•857
KCNS
0
•932
o
.868
0.8l4
KI
0.970
0
•942
0
.900
K2SO4
0
.875
o
.772
0.678
KOH
0.852
o
.716
o
.607
K2SO3
o
.865
o
.768
0.675
NaCl
0.938
o
.889
o
843
K2CO3
o
.788
o
.650
0-554
NaBr
0.965
0
.916
0.
890
K2C2O4
0
.866
o.
.771
0.675
Nal
0-995
o
.992
0.
985
K2CrO4
o
.866
o
.771
0.675
NaOH
0.876
0
.789
o.
7l6
CH3COOK
0
.866
o.
765
0.685
LiCl
0.980
I
.008
I.
045
HCOOK
0
.868
o.
760
0.678
LiBr
I .OOI
I
.040
I.
090
KBO2
o
,814
0.
677
0.560
Lil
1.030
I
.094
I .
190
K2HPO4
0.
860
o.
749
0.664
LiOH
0.863
0
.808
0.
768
Na2S
0.
887
0.
795
0.726
KF
0.839
0.722
p.
626
*KC1O3
0.927
KNO3
0.923
o
.862
o.
804
*KBrO3
o.
940
.
. .
. . .
KN02
0.920
0
.855
0.
798
*KIO3
0.
951
• .
* These salt solutions are 0.25 normal.
Konowalow (1898) expressed the results of determinations of the solubility
of ammonia in aqueous silver nitrate by the equation H = 56.58 (m — 2 n) in
which H = partial pressure of NH3 in mm. of Hg., m = molecular concentra-
tions of NH3 and n = molecular concentration of AgNO3. Similar results are
given in later papers (Konowalow, 1899, a, b) for a large number of other salt
solutions.
Gaus (1900) gives data for the vapor pressure of ammonia in aqueous 0.4 n
solutions of about 20 salts, only a few of which occur in the above table.
37 AMMONIA
SOLUBILITY OF AMMONIA IN ABSOLUTE ETHYL ALCOHOL.
(Delepine — J. pharm. chim. [5] 25, 496, 1892; de Bruyn — Rec. trav. chim. n, 112, '92.)
Gms. NHa Gms. NH3 per 100 Gms. Solution. Gms. NH3 per 100 Gms. Alcohol
t .
Density.
per 100 cc.
Solution.
(Delepine.)
(de Bruyn.)
(Delepine.)
(de Bruyn.)
o
0.782
13
•05
20
•95
19
•7
26
•5
24
•5
5
0.784
12
.00
19
.00
17
•5'
23
•o
21
.2
10
0.787
10
•8S
16
•43
15
.0
19
.6
17
.8
15
0.789
9
.20
13
.00
13
.2
15
• 0
15
.2
20
0.791
7
•5°
10
.66
II
•5
II
•9
13
.2
25
0-794
6
.00
10
.0
10
.0
II
.0
II
.2
30
0.798
5
•J5
9
• 7^
8
.8
10
•7
9
•5
According to Miiller (1891), one volume of alcohol absorbs 340 volumes of
ammonia at 20° and 760 mm. pressure.
SOLUBILITY OF AMMONIA IN AQUEOUS ETHYL ALCOHOL.
(Delepine.)
In 06% Alcohol. In 90% ^Alcohol. In 8o%AAlcohol.
t°. Sp. Gr. G. NH3 per
Solution, zoo Gms. Sol.
Sp. Gr.
Solution.
G. NH3 per *
100 Gms. Sol.
fc'Sp. Gr. G. NHS per
Solution. 100 Gms. Sol.
0
O
•783
24
•5
O
.800
30.25
0.8o8
39-o
10
0
.803
18
.6
0
•794
28.8
O.Soo
28.8
20
o
.788
14
.8
0
•795
15-8
0.821
19.1
30
o
.791
10
•7
O
.796
II-4
0.826
12.2
In 60%
Alcohol.
In so%_ Alcohol.
t .
Sp. Gr.
Solution.
G. NH3 p
100 Gms. S
.
Sp. Gr.
Solution.
G. NH3 per"
100 Gms. Sol.
0
0-830
50-45
0.835
69.77
10
0.831
37-3
0.850
43.86
20
0.842
26.1
0.869
33-8
30
0.846
21 .2
0.883
25.2
SOLUBILITY OF AMMONIA IN ABSOLUTE METHYL ALCOHOL.
(de Bruyn — Rec. trav. chim. n, 112, '92.)
0 G. NH3 per 100 Grams. 0 G. NH3 per^ioo Grams.
Solution. Alcohol. Solution. Alcohol.
O 29.3 41.5 20 19.2 23.8
5 26.5 36.4 25 16.5 20.0
10 24.2 31.8 30 14.0 16.0
15 21.6 27.8
SOLUBILITY OF AMMONIA IN ETHYL ETHER.
(Christoff, 1912.)
Results in terms of the Ostwald Solubility Expression (see page 227), at
o° = 17.13, at 10° = 12.35, at 15° = 10.27.
Freezing-point lowering curves (Solubility, see footnote, page i) are given
by Baume and Perrot (1910), (1914) for mixtures of ammonia and methyl
alcohol and for mixtures of ammonia and methyl ether; results for ammo-
nium and potassium, ammonium and sodium, and ammonium and lithium are
given by Ruff and Geisel (1906); results for ammonium and hydrogen sulfide
are given by Scheffer (1912).
SOLUBILITY OF AMMONIA IN HYDROXYLAMINE.
(de Bruyn, 1892.)
100 gms. of the sat. solution contain 26 gms. NH3 at ±0° and 19-20 gms. at
I50-i6°.
AMMONIA 38
DISTRIBUTION OF AMMONIA BETWEEN:
Water and Amyl Alcohol at 20°. Water and Chloroform at 20°.
(Herz and Fischer — Ber. 37, (Dawson and McCrae — J Ch. Soc. 79, 496, '01; see
4747. '04) also Hantsch and Sebaldt — Z.phys.Ch.ao, 258, '99.)
Cms . NHg per 100 cc.
G
. M. NHa per too cc.
Cms
. NHaper 100 cc.
G. M. NH3 per 100 cc.
' Aq.
Alcoholic
Aq.
Alcoholic
Aq.
CHC13
Aq.
CHCla
Layer
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
o-5
0.
.072
O
•25
O
•0035
O
.2
O.OO7
O.OI
0.00038
I 0
0
.147
O
•50
0
.0073
0
•4
0-015
0-02
0.00073
2 -O
O
.272
I
.00
0
.0148
0
.6
0.023
C.03
O.OOII4
30
0
438
2
• oo
0
-02Q5
O
.8
0.031
O.O4
O.OOI52
40
0
595
3
.00
O
• 0460
I
• o
0.039
O.O5
0.00193
5-°
0
•756
I
.2
0-046
0.06
0.00232
I
•4
0-055
0.08
O.OO3II
I
.6
0-063
o.io
0-00396
For calculations of above distribution results see Note, page 6.
Additional data for the distribution of ammonia between water and chloroform
are given by Dawson and McCrae (1900), (19010), (19016); Dawson (1906),
(1909); Abbott and Bray (1907); Sherrill and Russ (1907); Bell (1911), and
by Moore and Winmill (1912). The results show that with increase of concen-
tration of ammonia, the relative amount in the aqueous layer diminishes. Thus
Bell found that at 25° the distribution ratio is 22.7 when the aqueous layer con-
tains 1. 02 gm. mols. NH3 per liter and only 10 when 12.23 Sm- mols. NH3 are
present in the aqueous layer. The influence of increase of temperature was
also found to be in the direction of diminution of the relative amount in the
aqueous layer.
The influence of the presence of a large number of salts in the aqueous layer
has been studied by several of the above-mentioned investigators. In the case
of copper, zinc and cadmium salts (Dawson and McCrae, 1900), {Dawson, 1909),
the distribution ratio varied with salt concentration in a manner indicating that
metal ammonia compounds were formed.
Results for the effect of KOH, NaOH and Ba(OH)2 on the distribution at 18°
are given by Dawson (1909).
Results for the effect of ammonium chromate upon the distribution at 25°
are given by Sherrill and Russ (1907).
Results for the distribution of ammonia between water and mixtures of chloro-
form and amyl alcohol at 25° are given by Herz and Kurzer (1910).
DISTRIBUTION OF AMMONIA BETWEEN TOLUENE AND AIR.
(Hantzsch and Vagt, 1901.)
Gms. NHajrer 1000 cc. Mols. NHs per 1000 cc.
Air. C6H8CH3 Layer. Air.
o 0.366 0.0396 0.0215 0.00233
10 °-357 °-°435 0.0210 0.00256
20 0.326 0.0451 0.0192 0.00265
30 0.286 0.0462 0.0168 0.00272
39
AMMONIUM ACETATE
AMMONIUM ACETATE CH,COONH4.
100 cc. of sat. solution in acetone contain 0.27 gm. CH3COONH4 at 19°.
(Roshdestwensky and Lewis, 1912.)
AMMONIUM ARSENATES.
THE SYSTEM AMMONIA,; ARSENIC TRIOXIDE AND WATER AT 30°.
(Schreinemakers and de Baat, 1915.)
Gms. per 100 Gms. Sat. Sol.
NHj.
0
I.4I
2.78
2.86
2.88
2.26
10.98
20.49
21 .17
18-43
Solid Phase.
AsA
Gms. per 100 Gms. Sat. Sol.
NH3.
3-13
3-91
6-95
9-93
4.28
Data are also given for the system NH4C1
100 gms. H2O dissolve 0.02 gm. NH4CaAsO4.£H2O.
" " " " 0.014 " NH4MgAsO4.*H8O.
AS203.
12.30
7-63
4.72
3.20
2.16
+ H20 at 30°.
Solid Phase.
(Field, 1873.)
SOLUBILITY OF AMMONIUM MAGNESIUM ARSENATE IN WATER AND IN
AQUEOUS SOLUTIONS OF AMMONIUM SALTS.
(Wenger, 1911.)
Gms. NH4MgAsO4 per 100 Gms. of Each Solvent.
Solid Phase.
NH4MgAs04.6HzO
Water.
Aq. 5%
NH4N03.
Aq. 5%
NH4C1.
Aq.*
NH4OH.
NH4OH t
Aq.
NH4OH f
+10%
-vfrr pi
O
O
•0339
0.092
0
.084
0
.0087
...
JN±14C1.
20
0
.0207
0.
114
0
.113
0
.0096
0.013
0.032
30
0.
118
O
•113
40
0
.0275
0.
139
0
.190
0
.0117
50
o
.0226
0.
189
O
.189
0
.0100
• . .
...
60
O.O2IO
o.
211
0
.219.
0
.0090
0.047
0.054
70
0
.0156
0.
I89
0
.221
o
.0095
...
...
80
O
.0236
o.
189
O
.231
0
.0091
* Composed of i part NHt(4 = 0.96) + 4 parts KfeO.
t Contained 4 parts NHi(d = 0.96) per 100 parts NH4C1 solution.
AMMONIUM BENZOATE C.H,COONH4.
SOLUBILITY IN WATER AND IN AQUEOUS ALCOHOL AT 25°.
(Seidell, 1910.)
Gms. CzHsOH
per 100 Gms.
Solvent.
d& of Sat. Sol.
Gms.
C6H6COONH4
per 100 Gms.
Sat. Sol.
Gms. C2HsOH
per 100 Gms.
Solvent
0
1.043
18.6
60
10
I .027
18
70
20
1. 012
18
80
30
0.997
18.1
90
40
0.979
18
95
50
0.956
17
100
<fe of Sat. Sol.
Gnis.
C6H5COONH4
per 100 Gms.
Sat. Sol.
0.930 15
0.901 12.2
0.864 8.3
0.828 4.2
O.SlO 2.7
0.796 1.6
100 gms. water dissolve 19,6 gms. C6H5COONH4 at 14° 5, du of sat. sol. =
1.042. (Greenish and Smith, 1901.)
ioo gms. water dissolve 83.33 gms. C6H6COONH4 at b.-pt. (U. S. P.)
100 gms. glycerol dissolve 10 gms. C6HBCOONH4 at room temp. (Hager.)
AMMONIUM BORATES
40
THE SYSTEM AMMONIA, BORIC ACID AND WATER AT 30° AND AT 60°.
(Sborgi, 1913-15; Sborgi and Meccacci, 1916.)
Results at 30°. Results at 60°.
(NI
O
0
•23
.70
B
4
7
.81
.20
oana irnase.
Jtis-ljOs
n
(NH4)2O.
0
0.78
B203.
7-39
12.12
ouiiu .rua.se.
H3BO3
0
.78
7
.62
HJBOH- 1.5.8
I
.42
15-
60
H3B03+ 1.5.8
0
•99
7
•53
1.5-8
I
.70
15-
29
1.5-8 "
I
.08
7
.66
tt
3
•23
18.
60
a
I
.71
9
•13
"
4
.02
20.
38
1.5-8+1.
4.6
2
•25
10
tt
4
.88
21 .
76
1.4.6
2
.89
12
-32
It
6
.41
24.
32
"
3
•13
12
•59
tt
7
.90
27.
3i
1.4.6+1.
2.4
3
•43
6
•35
24.5
7
-83
26.
76
1.2.4
6
.51
4
48
tt
7
.91
17-
57
u
10
•45
3
•37
"
9
•57
13-
56
(i
18
•05
2
.02
11
15
•45
8.
33
(i
24.80
I
•51
"
19
•47
5-
92
"
30
-56
I
.22
(t
22
•57
4-
47
"
45
•34
0
.84
U
1.5-8
= (NH4)20,
,5B203.8H20
1.4.6 =
(NH4)20.4B203.6H20
2-4-5
= 2(NH4)20.4B203.5H02
1.2.4 =
(NH<
)20.2B203.4H20
AMMONIUM BROMIDE NH4Br.
SOLUBILITY IN WATER.
(Smith and Eastlack, 1916.)
(Determinations by sealed tube method.)
Gms. NH4Br
per too Gms. t°.
HzO.
107.8 130
116.8 137.3
126 140
135-6 150
145.6 160
156.5 170
167.8
SOLUBILITY OF AMMONIUM BROMIDE IN ABSOLUTE ETHYL ALCOHOL,
METHYL ALCOHOL, AND IN ETHER.
(Eder; de Bruyn — Z. phys. Ch. 10, 783, '92.)
Cms NH4Br
t°.
per 100 Gms.
t°.
H20.
— 17 Eutec.
47-3
60
0
60.6
70
10
68
80
20
75-5
90
30
83-2
£00
40
91.1
no
5°
99.2
120
Gms. NH4Br
per 100 Gms.
HzO.
1 80
Transition pt.
192.3
202.5
213.4
225-5
In Ethyl Alcohol.
Gms. NHiBr
per 100 Grams.
15
19
78
Solution.
2.97
3.12
9-50
Alcohol.
3.06
3-22
10.50
In Methyl Alcohol.
Gms
per 100 Grams.
Solution
II. I
Alcohol.
I2-5
In Ether (o 729 Sp. Gr.).
Gms. NHjBr
per 100 Grams.
Ether.
0.123
loo cc. ethyl alcohol of di6 = 0.8352 dissolve 7.8 grams NH4Br at 15°, di& of
sat. sol. = 0.8848. (Greenish, 1900.)
100 cc. anhydrous hydrazine dissolve no gms. NH4Br at room temp, with
evolution of ammonia. (Welsh and Broderson, 1915.)
4i AMMONIUM BROMIDE
SOLUBILITY. OF AMMONIUM BROMIDE AT 25° IN MIXTURES OF:
(Herz and Kuhn, 1908.)
Methyl and Ethyl
Alcohols.
Propyl and Methyl
Alcohols.
-A
Propyl and Ethyl
Alcohols.
t
Gms.
/"•*
Gms.
Gms.
Gms.
< Gms.
CHsOH per
zoo Gms.
Solvent.
Sat. Sol.
NH4Br
per 100
cc. Sat.
Sol.
CsHyOHper d ^ of
100 Gms. Sat. Sol.
Solvent.
NH4Br
per 100
cc. Sat.
Sol.
C3H7OH
per 100
Gms. Sol-
vent.
Sat. Sol.
NftBr
perioo
cc. Sat.
Sol.
0
0
.8065
2-55
0
0.8605
9.83
0
0.8065
2-55
4-37
0
.8083
2.99
II
.11
0.8524
8.51
8.
5i
0.8o62
2.51
10.40
o
.8117
3.2I
23
.8
0.8426
6.90
17-
85
0.8052
2-37
41.02
0
.8252
5.06
65
.2
0.8184
3.08
56.
6
0.8048
1.63
80.69
o
.8501
8.13
91
.8
o . 8097
1.28
88.
6
o . 8042
I. II
84.77
o
.8508
8.47
93
•75
0.8089
1-25
91.
2
o . 8049
I .05
91.25
0
.8551
9-34
100
0.8059
95-
2
o . 8059
1.04
100
o
.8605
9.83
100
0.8059
0.95
AMMONIUM Cadmium BROMIDE (NH4)CdBr3.|H2O.
100 parts water dissolve 137 parts of the salt; 100 parts of alcohol dissolve
18.8 parts and 100 parts of ether dissolve 0.36 part. (Eder, 1876.)
AMMONIUM Platinum BROMIDE (NH4)2PtBr6.
100 gms. sat. aqueous solution contain 0.59 gm. salt at 20°. (Halberstadt, 1884.)
SOLUBILITY OF TETRA ETHYL AMMONIUM BROMIDE N(C2H6)4Br, AND OF
TETRA METHYL AMMONIUM BROMIDE N(CH3)4Br IN ACETONITRILE.
(Walden — Z. phys. Ch., 55, 712, '06.)
100 cc. sat. solution in CH3CN contain 9.59 gms. N(C2H6)4Br at 25°.
100 cc. sat. solution in CH3CN contain 0.17 gm. N(CH3)4Br at 25°.
SOLUBILITY OF TETRA ETHYL AMMONIUM BROMIDE IN WATER AND
IN CHLOROFORM AT 25°.
(Peddle and Turner, 1913.)
loo gms. H2O dissolve 279.5 gms- N(C2H6)4Br.
100 gms. CHC13 dissolve 25.01 gms. N(C2Hs)4Br.
Data for the distribution of propyl benzyl methyl phenyl AMMONIUM
BROMIDE between water and chloroform at 25° are given by Wedekind and
Paschke (1910).
AMMONIUM CARBONATE (NH4)2CO3.
100 gms. H2O dissolve 25.4 gms. ammonium carbonate, calculated as
C2HnN3O5 at 16.7° d of sat. sol. = 1.095. (Greenish and Smith, 1901.)
100 gms. of carefully purified glycerol dissolve 20 gms. (NH4)2CO3 at 15°.
(Ossendowski, 1907.)
AMMONIUM BICARBONATE NH4HCO3.
SOLUBILITY IN WATER.
(Dibbits — J. pr. Ch. [2] 10. 417, '74.)
to Gms. NH4HCO3 per 100 Grams. Grams NlfrNCOa per 100 Grams.
Solution. Water. Solution. Water.
O 10.6 II-9 20 17.4 21.0
5 I2-i 13-7 25 J9 3 23.9
10 13.7 15.8 30 21.3 27.0
*5 iS-5 18.3
AMMONIUM BICARBONATE
42
SOLUBILITY OP AMMONIUM BICARBONATE IN AQUEOUS SOLUTIONS OP
AMMONIUM CHLORIDE SATURATED WITH CO2.
(Fedotieff — Z. phys. Ch. 49, 168, '04.)
Per 1000 cc. Solution.
Per 1000 Grams H2O.
o
Wt.OI
zee. Sol.
G.
NE
M.
uci.
G. M. Gms.
NEUHCOa- NEUCl.
Gms
NH4H
COa.
G.M.
NEUCl.
0.0
G.M.
NEUHCO
1.22
Gms.
3. NH4C1.
O*O
Gms.
NH4HCOj
II9.0
o
1.077
4
.41
0-37
235-9
29
.2
5-42
0.46
290.8
36.0
15
1.064
0
.0
2.12
0-0
I67
.2
o.o
2.36
o.o
186.4
15
1.063
0
•5
1.84
26.8
145
.2
0.56
2.06
29.9
162.9
15
I .062
I
.0
I .59
53-5
I25
•5
1.13
1. 80
60.6
142.2
15
I .062
I
.41
1.42
75-4
112
.2
i-59
1. 60
85.1
126.9
IS
1.065
I
.89
4.28
100.8
101
.1
2.18
1.48
II6.8
116.8
IS
1.069
2
-87
0-99
153-3
78
.2
3-42
1.18
183.0
93-3
IS
1.076
3
.84
0-79
205.2
62
•5
J-03
0.98
269.3
77-3
IS
1.085
4
.82
0.65
257-9
51
•4
6.21
0.84
332.5
66.4
IS
1.085
4
•95
O.62
264.8
48
•9
6.40
0.81
343-5
64.2
30
...
o.o
3-42
o.o
270.0
*o
...
7.4
1.1*
307. 0
oi.o
SOLUBILITY OF AMMONIUM BICARBONATE IN AQUEOUS SOLUTIONS OP
SODIUM BICARBONATE SATURATED WITH CO2.
(Fedotieff.)
Per 1000 cc. Solution. Per 1000 Grams H2O.
t°
Wt.
of
G.M.
G.M.
Gms.
Gms.
G.M.
G.
M.
Gms.
Gms.
I CC.
Sol.
NaHCO3. NH4HCO3.
NaHCOa. NHiHCOa-
NaHCOa.
NHiHCOs. NaHCO3.
NHiHCOg
O -O
I
. <\I'
o .0
110 -O
0
I.
072
o-53
1.28
44.6
IOI-4
0-58
I
0 A
•39
48.2
J.J.V/ -w
109.4
IS
I.
064
0.0
2.12
o.o
167.2
o.o
2
-36
o.o
186.4
15
I.
090
0.63
1.92
S2'5
I5I-3
0.71
2
.16
59-2
170.6
2n
o«o
.42
O-O
27O.O
3°
30
%
0.83
2
.01
7o.o
230.0
SOLUBILITY OF AMMONIUM BICARBONATE IN AQUEOUS SOLUTIONS OF
AMMONIUM NITRATE.
(Fedotieff and Koltuno'ff, 1914.)
d of Sat.
Gms. per 100 Gms. H2O.
t°
d of Sat.
Gms. per 100 Gms. HzO.
.
Sol.
NH4NO3.
NH*HCO3.
w •
Sol.
NH4NOs.
NH4HCOs.
0
O
11.90
IS
1.242
103.4
8.25
o
1.265
1x8
4-52
IS
1.269
128.9
7-79
15
1.064
o
18.64
15
1.302
166.9
7.46
15
I.H3
23.26
12.91
30
0
26.96
15
1.164
49-82
10-33
30
...
231.9
12-57
43
AMMONIUM BICARBONATE
SOLUBILITY OF MIXTURES OF AMMONIUM BICARBONATE,
BICARBONATE, AND AMMONIUM CHLORIDE IN WATER
SATURATED WITH CO2.
(Fedotieff.)
SODIUM
*«, *Wt. of
* * » *•*• C*-J
Gram Mols. per
Gms. H2O
IOOO
Gms. per 1000 Gms. HgO.
Solid
pu___
I CC. oOJ
o 1.114
' NaHC03.
0-59
NaCl.
0.96
4.92
NaHCOa.
49.61
NaCl.
56.16
NHiC
263.
4
rnase.
a+b-h
o 1.187
0-12
4-83
2.74
10.
09
282
.6
146.
7
"
15 1.116
o-93
0.51
6.28
78.
18
29
.84
'336.
2
"
15 1.178
0.18
4.44
3-73
15
*3
259
.8
199.
6
M
15 1.151
0.30
3-09
4-56
25-
22
180
.8
244.
i
a + c
r5
.128
0.51
1.68
5-45
42.
87
98
.28
291 .
7
"
15
.112
0.99
o-35
5-65
83-
22
20
•47
302.
4
a + b
J5
.108
1.07
0.20
5.21
89.
95
ii
.70
278.
9
"
.106
I .12
o.n
4.92.
94-
14
6
•44
263.
4
'*
15
.101
1.16
0.14
4.00
97-
52
8
.19
214.
i
M
15 i .090
o-93
0-95'
2.03
78.
18
55
•58
108.
6
M
a =
NaHC03
b =
NH
'V-/3j
c
-
NH4C1.
AMMONIUM Uranyl CARBONATE 2(NH4)2CO8UO2CO3.
(Ebelmen.)
100 grams H2O dissolve 5 grams of the salt at 15°...
AMMONIUM Lead COBALTICYANIDE NH4PbCo(CN)6.3H2O.
(Schuler — Sitz. Ber. K. Akad. W. (Berlin) 79, 302.)
100 grams H2O dissolve 12 grams of the salt at 18°.
AMMONIUM PerCHLORATE NH4C1O4.
SOLUBILITY IN WATER.
(Carlton, 1910.)
Sp Gr
Gms. NH4C1O4
t°.
Sat. Sol.
per 100 cc.
Sat. Sol.
o
1.059
11.56
20
1.098
20.85
40
I.I28
30.58
60
I.I58
39-05
t°
Sp. Gr.
Sat. Sol.
Gms. NH4CKX
per TOO cc.
Sat. Sol.
80
I-I93
48.19
100
1.216
' 57-01
107 b. pt.
I. 221
59.12
.In a paper by Thin and Gumming (1915), it is stated that ammonium per-
chlorate is "sparingly soluble" in water and according to one determination
at 14.2°, 100 gms. of the sat. solution was found to contain 1.735 gms. NH4C1O4.
It is probable that these authors have misplaced the decimal point. This ap-
pears more probable since a determination of the solubility in 98.8 per cent
ethyl alcohol at 25.2° gave 1.96 gms. NH4C1O4 per 100 gms. sat. solution, and
in 98.8 per cent alcohol containing 0.2 per cent HC1O4 gave 1.97 gms. per 100
gms. sat. solution.
AMMONIUM PerCHLORATE
44
SOLUBILITY OF AMMONIUM PERCHLORATE AND SEVERAL OF ITS DERIVATIVES IN
WATER AT 15°. (Hofmann, Hobald and Quoos (1911-12).)
Gms. Salt per Gms. Salt per
100 Gms. H2O. 100 Gms. H2O.
18.5 CH3(C2H5)3NC1O4 23.6
109 . 6 C3H7(C2H5)3NC1O4 7 . 9
208.7 (CH3)2(C2H5)2NC104 134.3
208.7 C2H3(CH3)3NC104 5
150.9 BrCx2H4(CH3)3NClO4 3-5
1 9 . 9 BrC2H2(CHs)2NC104 2 . 5
'0.5 (OH)C2H4(CH3)3NC1O4 290.7
3.7 (OH)CH2CH(OH)CH2(CH3)3NC104 155 . 7
17.9 NO3C2H4(CH3)3NC104 o . 6
3.1 C3H5(CH3)3NC104 199.5
10.9 C2H4(NH3C1O4)2 144.5
15.4 C2H4[(CH3)3NC104]2 ,1.2
3.7 C3H6[(CH3)3NC104]2 1.5
2.2 Br2C2H3(CH3)3NClO4 2.2
BrC3H3(CH3)3NClO4 2.6
Milbauer (1912-13) found that 100 gms. of cold H2O dissolve 1.126 gm. tetra-
methyl ammonium perchlorate (CH3)4NC1O4 and 100 gms. alcohol dissolve
0.04 gm. of the salt.
AMMONIUM CHLORIDE NH4CL.
SOLUBILITY IN WATER.
(Mulder; below o°, Meerburg — Z. anorg. Ch. 37, 203, 1903.)
CH3NH3C104
(CH3)2NH2C1O4
C2H5NH3C1O4
(C2H5)2NH2C1O4
(CH3)3NHC1O4
(CH3)4NC104
(C2H5)4NC104
C6H5(CH3)3NC1O4
ICH2(CH3)3NC1O4
C2H5(CH3)3NC1O4
C3H7(CH3)3NC104
C5H11(CH3)3NC1O4
Gms. NHjCl per 100 Gms.
Gms. NH4C1 per too Gms.
» .
Solution.
Water.
-IS
19.7
24-5
— 10 9
20-3
25-5
~5-7
21-7
27.7
0
22-7
29.4
+ 5
23-8
31.2
10
24.9
33-3
15
26.0
35-2
20
27.1
37-2
25
28.2
39-3
30
29-3
41.4
m .•
Solution.
Water.
40
31-4
45-8
50
33-5
5° 4
60
35-6
55-2
70
37-6
60.2
80
39-6
65.6
90
41 .6
7i-3
100
43-6
77-3
no
45 -6
83.8
115.6
46.6
87-3
Density of saturated solution at o° = 1.088, at 15° = 1.077, at 19° = I-°75-
Eutectic, Ice + NH4C1 = — 16° and 19.5 gms. NH4C1 per 100 gms. sat. sol.
100 gms.. H2O dissolve 31.25 gms. NH4C1 at 3.5°, 38.5 gms. at 25° and 49.6
gms. at 50°. (Biltz and Marcus, 1911.)
Data for the solubility of ammonium chloride in water at o° under pressures
up to 500 atmospheres are given by Stackelberg, 1896.
SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS AMMONIUM BICARBONATE SO-
LUTIONS SATURATED WITH CO2. (Fedotieff— z. Phys. Ch. 49, 169, 1904.)
Per 1000 cc. Solution.
Per 1000 Gms.
t<>.
Wl. 01
i cc. Sol.
G.M.
NHJICOa.
G. M.
NH4C1.
Gms.
NH4HCO
Gms. ''
O
1.069
0-0
4.60
o.o
246.1
O
15
IS
2O
1.077
1.077
1.085
o-37
o.o
0.62
4.41
5-29
4-95
29.2
O-O
48.9
235-9
283.1
264.8
J°
•?r»
G. M. G. M. Gms. Gms.
NH4HC03. NH4C1. NH4HC1. NEUCl.
o.o 5.57 o.o 298.0
0.46 5.42 36.0 290-8
O.O
0.8l
0-0
6.64 o.o
6.40 64.2
7.78
355-Q
343-5
416.4
7.40 91.0 397. o,
o.o
45 AMMONIUM CHLORIDE
SOLUBILITY IN AQUEOUS AMMONIA SOLUTIONS AT o°.
(Engel — Bull. soc. chim. [3] 6, 17, 1891.)
Milligram Molecules Grams" per 100 cc.
Sp. Gr. of per 10 cc. Solution. Solution.
SolUtionS. TT— ' f VrTrp.tr ' MTT ri
JNiia. JNrUd. XMJtliUxl. JNli^Ll.
1.067 5.37 45-8 0-92 24.52
1.054 12-02 45.5 2.05 24.35
1.031 38.0 44-5 6-48 23.82
1.025 47.0 44-o 8.02 23.56
1-017 54-5 43-63 9-30 23.35
0.993 80.0 43-12 13-66 23.09
0.992 90.0 44.0 15-36 23.56
o-983 95-5 44-37 l6-29 23.75
o-953 J3Q o 49-75 22-i8 26.63
0.931 169.75 60.0 28.97 32.14
SOLUBILITY OF NH4C1 IN AQUEOUS AMMONIA SOLUTIONS AT 17.5°.
(Stromholm, 1908.)
Normality Equiv. per Liter. Gms. per 1000 cc. Solution.
' NH3. NH4C1. ' ' NH3. NH4C1."
o 5.435 o 290.8
0.15 5.420 2.55 290
4.76 5.082 81 271.9
SOLUBILITIES OF MIXTURES OF AMMONIUM CHLORIDE AND OTHER SALTS
IN WATER.
(Riidorff, Karsten, Mulder.)
Both salts present in solid phase;
te Grams per 100 Grams HgO. to Grams per 100 Grams H2O.
19.5 29 . 2 NH4C1+ 1 74 . o NH4N03 * R b. pt. 67.7 NH4C1+ 21.9 KC1 M
21.5 26.8 " + 46.5(NH4)2SO4R 14-8 38.8 " +34-2KNO3K
20.0 33.8 " + ii.6BaC!2 R 18.5 39.8 " +38.6KNO3K
18.5 39.2 " + i7.oBa(NO3)2 K 14.0 36.8 " +i4-iK2SO4R
15.0 28.9 " + 16.9 KQ R 18.7 37.9 " +i3.3K2S04K
22.0 30.4 " + i9.iKCl R iS.f 22.9 -f-23.9NaCl R
SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM
SULFATE AT 30°.
(Wibaut, 1909; Schreinemakers, 1910.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
tNHO.504. ' NH4C1. - SolldPhase- '(NH4),S04. ' NH.C1. ' Sohd Phase.
o 29.5 NH4C1 25 18.3 NH4C1+(NH4)2S04
5 28.5 30 13.2 (NH4)2SOi
10 25.7 35 8.5
15 23.2 40 2.8
20 20.2 " 42 O
SOLUBILITY OF MIXTURES OF AMMONIUM CHLORIDE AND COBALT CHLORIDE
IN WATER AT 25°. *
(Foote, 1912.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Solid Residue.
Solid Phase.
Mixed crystals of
NH4Cl+CoCl2.
2H2O
Mixed crystals +
CoCl2.6H2O
NH4C1. CoCl2. NH4C1. CoC!2. H2O.
17.90 15.63 ... 3.2
13-59 25.19 83.01 13.52 3^7
8.75 34.28 35.12 50.66 14.22
7-45 35-24 34-02 49.64 16.31
7.62 34.61 7.07 55.27 37.66
AMMONIUM CHLORIDE
46
SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS HYDROCHLORIC ACID.
Results at O°. (Engel, 1888.)
So Gr. of Sat. Gms- P** I0 cc- &&• so1-
Sol.
.076
.069
.070
•073
.078
.106
.114
HCl.
i.99
3-93
7-74
19. i8
22.07
NH4C1.
24.6l
23.16
21.78
19.36
14-54
5-78
4.67
Results at 25°. (Armstrong and Eyre, 1910-11.)
Gms. HC1 pe
too Gms. H2(
O
O.QI
1.82
3.65
18.25
d $f Gms. NIL.C1 per
Sat. Sol. 100 Gms. Sat. Sol.
.080
28.3
.079
.082
•083
27.4
26.4
24.6
.099
n-3
SOLUBILITY OF MIXTURE OF AMMONIUM CHLORIDE AND LEAD CHLORIDE IN
WATER AT SEVERAL TEMPERATURES.
(At 17°, 50° and 100° Demassieux (1913) at 25° Foote and Levy, 1907.)
At 23°. At 50°. At 100°
At 17°.
Solid Phase
Gms.'per 100 Gms. Sol.
Gms. per 100 Gms. Sol.
Gms. per 100 Gms. Sol.
Gms. per 100 Gms.Sol.
in Each
fPbCl,.
NH4C1.
PbCl2.
NH.C1. *
' PbCl2.
NH4C1. '
PbCJ2.
NH4C1. "
Case.
0.30
27
•03
...
...
0.32
34
.14
1.61
43
.42
NH4C1
0.52
26
.68
. . .
. . .
2.65
33
.62
4.21
42
.91
"
0.64
26
•49
I. 2O
28.15
3.96
33
•56
. . .
.
. .
" +1.2
0.26
41
.00
" +2.1
7
9.88
T^
v/v
.22
2.1
II .60
38
.^2
12.67
o
37
o
.62
" +1.2
0-34
22
•32
0-93
27-45
3-31
31
.90
/
11.40
O 1
36
.29
1.2
0.098
12
•36
o-35
21-59
1.76
27
.16
8.32
32
.64
"
0.078
4
•93
0.29
17.97
0.71
19
.42
4-54
26
.08
•
0.078
4
•23
O.II
10.25
0.49
12
•45
1.98
13
.12
"
0.076
3-48
0.03
2-77
0.48
4
.86
1.76
8
•59
" +PbCl,
0.16
I
•43
...
0.67
I
•45
1.85
5
•33
PbCl2
0.21
0
.96
. . .
. . .
1. 08
o
2.02
i
•32
"
0.89
0
1.69
0
3.10
0
"
Gm. Equiv. Gm. Equiv. PbCla
NH4C1 per
iooGms.H2O.
per TOO Gms.
Sat. Sol.
° i
^.49 Xio-3
o.i ';
5.10 Xio-3
O.2
.9i6Xio-3
0.4 '
. 348XIQ-3
0-5 '
. 263 X lo"8
o-55
. 189X10-3
[0.6
.092X10-3
0.7 <
). 956X10-3
Solid Phase.
PbCl2
Solid Phase.
2PbCl2.NH4Cl
1.2 = NH4C1.2(PbCl2X 2.1 = 2NH4Cl.PbCl2.
The following additional data for the above system at 22° are given by Bron-
sted (1909).
Gm. Equiv. PbCl2
per 100 Gms.
Sat. Sol.
0.837XIO-3
0.758XIO-3
0.695XIO-3
0.968X10-3
I . 502 X I0~3
2.338X10-3
3.580XIO-3
Gm. Equiv.
NH4C1 per
100 Gms. H2O.
0.8
i
2
3
4
6
7. 29 sat. 6.46 Xio"
+NH4C1
YThe two curves intersect at 0.52 normal NH4C1.
SOLUBILITY OF MIXTURES OF AMMONIUM CHLORIDE AND MAGNESIUM CHLORIDE
IN WATER. (Biltz and Marcus, 1911.)
„ Gms. per loo Gms. Sat, Sol. „....,. *<> Gms. per 100 Gms. Sat. Sol.
*' ' MgCl2. " NH4C1. ' ^ - MgCl, NH4C1,
3-5 21.41 5.93 NH4Cl+MgCl2.6H20 3.5 34.43 0.09
25 20.95 8.78 " 25 35.41 0.09
50 20.84 12.46 " 50 36-92 0.15
47
AMMONIUM CHLORIDE
SOLUBILITY OF MIXTURES OF AMMONIUM AND MANGANESE CHLORIDES' IN
WATER AT 25°.
(Foote and Saxton, 1914.)
Cms, per 100 Gms. Sat. Sol.
NH4C1.
23-97
22.94
MnCl2.
7.97
9.65
21.44
21. 18
12.31
13.38
20. 10
I5-I9J
19.70
\
19.75
19.67
15-47]
Solid Phase.
a mixed crystals
Cms. per 100 Cms. Sat. Sol.
NH4C1.
MnCl2. '
17.09
18.76
15.05
22.44
13.17
9.15
24.52
29.24
ft mixed crystals or
double salt 2NH4C1.
MnCl2.2H2O
5.90
34.78
3-77
39.48
2.98
43.71
2NH4Cl.MnCl2.2H,O
2.94
43-44
+MnCl2.2H20
a mixed crystals consist of NH4C1 with varying amounts of MnCl2.2H2O;
/3 mixed crystals consist of the double salt 2NH4Cl.MnCl2.2H2O with excess of
NH4C1.
This case represents a very rare type of solid solution "in which a single salt
and a double salt are each capable of taking up very considerable quantities of
the other to form homogeneous mixed crystals."
EQUILIBRIUM IN THE SYSTEM AMMONIUM CHLORIDE, MERCURIC CHLORIDE,
WATER AT 30°.
(Meerburg, 1908.)
Gms. per 100 Gms. Sat. Sol.
' HgCl2.
NH4C1.
0
29.50
22.80
26.91
42.45
25-05
50.05
24-79
53-08
22.77
58.90
20.02
56.38
18.50
55.58
16.82
57-01
14.12
56.26
13.04
Solid
Phase.
Gms. per 100 Gms. Sat. Sol.
NH4C1
+1.1.1
1 +3-2.1
3-2.1
1.2.1 = HgCl2.2NH4Cl.H2O; i.i.i = HgCl2.NH4Cl.H2O;
3.2.1 = 3HgCl2.2NH4Cl.H2O; 9.2 = 9HgCl2.2NH4Cl.
* In these solutions 2 to 3 weeks were required for attainment of equilibrium.
' HgCl2.
NHjCl.'
57.05
9.92
58.65
9.20
*5i-83
8.76
*46
7.52
*35-6o
5.26
*32.90
5-06
29.65
3.62
40.12
5.13
21
2.29
7.67
0
Solid
Phase.
3-2.1
+9-2
+HgCl2
HgCl2
SOLUBILITY OF MIXTURES OF AMMONIUM AND NICKEL CHLORIDES IN WATER
AT 25°.
(Foote, 1912.)
Gms. per 100 Gms. Sat. Sol.
NH4C1.
NiCl2. '
26.07
3.10
22.27
8.04
20.68
10.32
Mixed crystals of
17-43
11.22
I5.OI
26.93
NH4C1 and
NiCl2.2H20
IO.2I
30.56
Q.l6
35.70
Gms. per 100 Gms. Sat. Sol.
Solid Phase.
NH4C1.
NiCl2.
7.98
37-41
8.07
37.73
Mixed crystals and
8.23
37-45
NiCl2.6H2O
8.17
37.64
7.51
37.191
3-06
37.98| NiCl,.6H20
O
37.53U
AMMONIUM CHLORIDE 48
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND AMMONIUM
CHLORIDE IN WATER AT 25°.
(Fock — Z. Kryst. Min. 28, 353, '97-)
Grams per Liter
Solution.
Mol. per cent
in Solution.
Sp. Gr. of
Mol. per cent in
Solid Phase.
' NH4C1.
KCl.
NHiCl.
KCl."
•Solutions*
NHtCi.
KCl.
o.oo
311-3
o.oo
IOO-O
1.1807
o.o
100
22. Si
293.3
9.41
90.59
1.1716
1. 21
98.79
35-39
278.7
15.04
84.96
1.1678
2. II
97.89
89.17
273.2
34.26
65-74
1.1591
6.18
93-82
127.8
234.6
46.59
53-44
1-1493
8.90
91.10
147.2
204.2
5I-63
48.37
1.1461
Jo- 53
89.47
197-3
157.7
63.56
36-44
1.1391
17.86
82.14
232.5
116.8
73-49
26.51
1.1326
60.20
39-80
244.5
123.0
73-48
26.52
1.1329
76.88
23.12
261.9
III.O
79.10
20.90
1.1245
97-51
2.49
259.0
102.2
82.14
17.86
I.I2I2
97-79
2.21
278.6
53 -16
87.96
12.04
I.I009
98.85
^S
320.7
31-24
93-45
6-55
I.09I2
99-33
0.67
273-5
o.oo
100.00
o.oo
1.0768
100 .0
o.oo
The following additional data for the above system are given by Biltz and
Marcus (1911). The results show that NH4C1 + KCl form a series of mix-
crystals broken by a gap which extends between about 20 and 98 mol. per cent
NH4C1 in the crystals.
Composition of Sat. Solution. Composition of Solid Phase.
Gms. per icx) Gms.
Mols. per 1000 Mols.
Gms. per 100 Gms. Mnl <£,
Sat.
Sol.
H,0.
Crystals.
NH4C1 in
NH4C1.
KCl.
NHiCl.
KCl/
NHtCl.
KCl.
Crystals.
5-13
22 .29
23.8
74.2
I. 21
98.79
1.7
7
20.40
32.5
67.9
2.22
97.78
3.1
ii
18.04
52.2
61 .4
4
96
5-5
13-73
16.11
65.9
55-5
5.89
94.11
8
15.46
14-53
74.4
50.2
7-24
92.76
9.8
19.54
12. l6
96.3
43
II .20
88.80
14.9
22.04
10.49
109
37-4
16.90
83.10
22.1
21.68
10.40
109
37-4
26.04
73.96
32.9
21.95
10.48
109
37-4
97.60
2.40
98.3
24.30
6.48
1x8.2
22.6
98.28
1.72
98.8
These authors also give data for the ammonium chloride carnellite and
potassium chloride carnellite diagram at 25°.
SOLUBILITY OF MIXTIJRES OF AMMONIUM AND POTASSIUM CHLORIDES IN WATER
AT 25°, 65° AND 90°.
(Uyeda, 1912.)
The results as presented by Uyeda show the percentage composition of the
dissolved mixture and of the undissolved residue in the several cases, but not
the quantity of salts dissolved. Mixed crystals were formed over certain ranges
of concentration at each temperature.
Data for the cryohydric temperatures and composition of the saturated solu-
tions of mixtures of the chlorides, nitrates and sulfates of ammonium, potas-
sium and sodium are given by Mazatto (1891).
49
AMMONIUM CHLORIDE
SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS {SOLUTIONS or
SODIUM CHLORIDE SATURATED WITH CO2.
(Fedotieff.)
Per 1000 cc. Solution.
Per 1000 Cms. H2O.
t°. Wt.of
G. M.
G. M.
Cms.
Gms.
G. M.
G. M.
Gms.
Gms.
i cc. Sol.
NaCl.
NH4C1.
NaCl.
NH4C1.
NaCl.
NHiCl.
NaCl.
NH4C1.
0
.069
0-0
4.60
0
.0
246
.1
o.o
5-57
o.o
298.0
O
.185
4.04
2.26
236
•5
121
.0
4.89
2-73
286.4
146.1
15
.077
0-0
S-29
O
•o
283
.1
o.o
6.64
o.o
355-Q
15
.097
0.81
4.71
47
•5
252
.1
1.02
5-91
59-8
316.4
15
.120
1.68
4-13
98
.0
221
•7
2.09
5-i8
122.4
277.0
15
•*S3
2.87
3-38
168
• o
180
•7
3-57
4.20
208.9
224.7
15
•175
3-65
2.98
213
•5
159
•4
4-55
3-72
266.8
198.8
30
o.o
7.78
0-0
416.4
30 1.166
3-30
3-70
J93
• o
I98
.0
4.26
4-77
249.0
255-4
45 •••
o.o
9-03
o-o
483.7
AC
4-0
6.02
233.9
322.1
SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS ETHYL ALCOHOL AT 15° AND
AT 30°.
Gms. C2HfiOH per
joo Gms. Solvent. '
ms. NELjCl per 100 C
ims. Solvent at:
15°.
30°.
0
35-2
40.4
20
40
60
80
25
16.8
9-5
4
29.7
19
5-3
92.3
100
0^6
. . .
Results at 15° by interpolation from Gerardin
;Bruyn (1892). Those at 30° from Bathrick (185
(1865), Greenish
,6).
(1900) and
100 gms. absolute methyl alcohol dissolve 3.35 gms. NH4C1 at 19°.
100 gms. 98% methyl alcohol dissolve 3.52 gms. NH4C1 at 19.5°.
(deBruyn, 1892.)
SOLUBILITY OF AMMONIUM CHLORIDE IN MIXTURES OF SEVERAL ALCOHOLS
WITH WATER.
(Armstrong, Eyre, Hussey and Paddington (1907); and Armstrong and Eyre (1910-11.)
Gm. Mols. Al- Gms. NH4C1 per 100 Gms. Sat. Solution in:
Gms. H2O.
Aq. CH3OH.
Aq. CjHsOH.
Aq. C3H7OH.
O
0
23
23
23
0
o
•25
22
.8
22
.6
22.
7
0
0
•50
22
.6
22
.2
22.
3
O
I
22
.1
21
•5
21.
i
0
3
20
•5
19
. .
25
0
28
•3
28
•13
(1.0805)
28.
3
25
0
•25
28.1
28
(i
.0780)
28.1
25
0
•50
27
•9
27
.6
d
•0753)
27.
5
25
I
27
.6
27
d
.0704)
26.
6
25
3
26
.1
26
•5
d
.0528)
. .
25
5
... 22.6
d
.0376)
(Figures in parentheses show Sp. Gr. of sat. sols.)
AMMONIUM CHLORIDE
SOLUBILITY OF AMMONIUM
CHLORIDE IN SEVERAL ALCOHOL MIXTURES AT 25°.
(Herz and Kuhn, 1908.)
In Methyl and Ethyl
Alcohol.
In Methyl and Propyl
Alcohol.
In Propyl and Ethyl
Alcohol.
Cms. CH3OH
per 100 Gins.
Solvent.
Cms. NH4C1 per
loo Gms. Sat.
Solution.
Gms. C3H7OH
per 100 Gms.
Solvent.
Gms. NH4C1 per
100 Gms. Sat.
Solution.
Gms. C3H,OH
per loo Gms.
Solvent.
Gms. NH4C1"
per 100 Gms.
Sat. Solution.
0
o-53
0
2.76
0
o-53
10
0.67
IO
2-33
10
0.50
20
0.80
20
1.90
20
0.47
30
0.98
30
1.58
30
0.42
40
1.18
40
1.26
40
o-39
50
1.40
50
1.03
5°
0.36
60
1.65
60
0.82
60
0.32
70
1.92
70
0.60
70
0.30
80
2.18
80
0.41
80
0.26
00
2.48
90
0.30
90
O.22
100
2.76
100
0.18
100
0.18
SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS GLYCEROL SOLUTIONS AND
IN AQUEOUS ACETONE SOLUTIONS AT 25°.
(Herz and Knoch — Z. anorg. Chem. 45, 263, 267, '05.)
In Aqueous GlyceroL
(Sp. Gr. of Glycerine 1.255, Impurity about 1.5%.)
Wt.%
Glycerine.
O.
13.28
25.98
45-36
54-23
83.84
IOO-OO
NHiCl per
Soluti
'Millimols"
585-I
544-6
502.9
434-4
403-5
291.4
228.4
tion.
Grams.
29.16
26.93
23 .26
21. 60
15.60
12.23
Sp. Gr,
at £
I .0793
1.0947
I.II27
I.I452
I .1606
1.2225
1.2617
Vol.%
O
10
20
30
40
*S
90
In Aqueous
NH4C1 per too cc.
S 1 tion.
Acetone.
Sp. Gr.
at-^--
1.0793
r.o6i8
1.0451
1.0263
0.9998
o . 9800
0.8390
0.8274
L indicates
L
U
jepa
MHlimols» Grams.
585-1 3I-32
534-1 28.59
464.6 24.87
396.7 21.23
328.5 17-59
283.7 15.19
18.9 i. oi
9-4 0.50
rates into two kyers.
lower layer, U indicates upper layer.
ioo cc. anhydrous hydrazine dissolve 75 gms. NH4C1 at room temp, with
evolution of ammonia. (Welsh and Broderson, 1915.)
SOLUBILITY OF TETRA ETHYL AMMONIUM CHLORIDE N(C2H5)4C1, AND
ALSO OF TETRA METHYL AMMONIUM CHLORIDE N(CH3)4C1 IN ACETONITRILE.
ioo cc. sat. solution in CH3CN contain 29.31 gms. N(C2H5)4C1 at 25°.
ioo cc. sat. solution in CH3CN contain 0.265 gms. N(CH3)4C1 at 25°.
(Walden — Z. physik. Chem. 55, 712, '06.)
SOLUBILITY OF TETRA ETHYL AMMONIUM CHLORIDE IN WATER AND IN
CHLOROFORM.
(Peddle and Turner, 1913.) ' « •
ioo gms. H2O dissolve 141.0 gms. N(C2H5)4C1 at 25°.
ioo gms. CHC13 dissolve 8.24 gms. N(C2H5)4C1 at 25°.
SOLUBILITY OF DIMETHYL AMMONIUM CHLORIDE IN WATER AND IN
CHLOROFORM.
(Hantzsch, 1902.)
ioo gms. H2O dissolve 208 gms. of the salt.
ioo gms. CHC13 dissolve 26.9 gms. of the salt (temp, not stated in abstract).
51 AMMONIUM CHROMATE
AMMONIUM CHROMATES.
SOLUBILITY IN WATER AT 30°.
(Schreinemaker — Z. physic. Chem. 55, 80, '06.)
Composition in Wt. per cent of:
' The Solution. The Residue/ Solid Phase-
% CrO3. % NH3. % CrO3. % NH3.
6.933 22.35 (NH4)2Cr04
9.966 16.53 47-59 20.44
16.973 8.20
22.53 6.37 38.03 12.15
27.09 6.87 48.02 12.01 (NH4)2CrO4+(NH4)2Cr2O,
26.19 5-7o 47-38 8.81 (NH4)2CraO?
25-99 5-10 4i -56 7-58
30.16 3.50
38.89 3.10 61.08 8.80
42.44 3-i5 59-72 6.75 (NHOAsO^CNHOaCrAu
44.08 2.27 54.90 4-14 (NH4)2Cr3O10
52.91 i. i i 60.88 3-09
54.56 1.03 63.07 3.09 (NH4)2Cr3O10+(NH4)2Cr4Olt
56.57 0.97 65.70 2.95 (NH4)2Cr4O3
58.87 0.65 69.74 3.24
62.48 0.46 71.93 3-10
63.60 0.40 73-68 1.18
63.66 0.41 71.47 2*.o;
62.94 0.21 CrOa
62.28 o.o CrO»
too gms. of the sat. aq. solution contain 28.80 gms.(NH4)2CrO4 at 30°.
100 gms. of thesat. aq. solution contain 32. 05 gms. (NH4)2Cr2O7at 30°.
AMMONIUM CITRATES.
SOLUBILITY IN AQUEOUS SOLUTIONS OF CITRIC ACID AT 30°.
(van Itallie, 1908.)
(Data read from curve plotted from original results.)
Gms. per too Gms. Sat. Sol.
• C.HA. ' NH3. ' SohdPhase-
65 O C,HA.H20
68 0.5
72 1.3
75 2.3 C6HA.H20+C6H7Q,
70 2.4 C6H7O7.NH4
65 2.5
60 2.7
55 2.8
52 2.8
50 3-6
49-2 5.1
50 6.2
Composition of the solid phases determined by " Rest Method."
(Schreinemakers, Z. anorg. Ch. 37, 207.)
AMMONIUM CALCIUM FERROCYANIDE.
100 gms. sat. aqueous solution contain 0.258 gm. (NH4)2CaFe(CN)6 at 16°.
(Brown.)
AMMONIUM FLUOBORIDE NH43BF3.
100 parts of water dissolve 25 parts salt at 16°, and about 97 parts at b. pt.1
(Stolba — Chem. Techn. Cent. Anz. 7, 459 )
,53
56
54
NH3.
7-5
8.2
8.5
8.5
— ^ OU11U JTUO3C.
C.HA.NH4
C6H707NH4+C(1H»07(NH<),
50
45-8
7-9
8.4
"
47
ii. i
"
50
12.9
c HA(NH!),+C«HA
54-5
14.5
6 (NHJj.p'HjO'
52
50
48.4
15
16
17.9
It
AMMONIUM FORMATE
AMMONIUM FORMATE HCOONH4| and also Ammonium Acid Formate.
SOLUBILITY IN WATER.
(Groschuff — Ber. 36, 4351, '03.)
to
Gms. HCOONH
4 per ioo Gms. Solid +0
Gms. per ioo Gms. Solution. Solid
.
Solution.
Water.
Phase.
HCOONH2. HCOOH
. ' Phase.
— 20
4I
•9
72
HCOONH4 — 6
•5
46
•7
34
.1
HCOONH4.HCOOH
0
50
•5
102
+ I
•5
49
.6
36
.2
"
20
58
•9
143
6
51
•3
37
•4
*
40
67
.1
204
8
•5
52
.1
38
*
60
75
-7
311
~~ 7
49
.6
36
.2
HCOONH4 labil.
80
84
.2
531
" +13
53
38
.6
"
stabil.
116
m.pt.
29
55
.8
40
•7
"
"
39
57
.8
42
.2
H2O free solution
SOLUBILITY OF AMMONIUM FORMATE IN FORMIC ACID SOLUTIONS.
(Groschuff.)
30 grams of HCOONHU dissolved in weighed amounts of anhydrous formic
acid and cooled to the point at which a solid phase separated.
Gms.
to HCOONH,
per ioo Gms.
Solution.
G. M.
HCOONH4 Solid
penooG.M. Phase.
HCOOH.
Gms. G. M.
to HCOONH4. HCOONH,
per ioo Gms. per ioo G.M
Solution. HCOOH.
Solid
Phase.
- 3
35-3
~n n HCOONH,
39-9 HCOOH
II
50
73 HCOONHi labil.
+ 8
•5
40.6
49.9
39
57-8
IOO
stabil.
21
•5
50
73
78
73-1
199
" "
Il6 m.pt.
IOO
00
•i «
ioo gms. 95% Formic Acid dissolve 6.2 gms. HCOONH4 at 21°. (Aschan, 1913.)
AMMONIUM IODATE NHJO3.
SOLUBILITY IN AQUEOUS IODIC ACID AT 30°.
(Meerburg, 1905.)
Gms. per ioo Gms. Sat. Sol.
—HIO; NHJOT SolidPhase-
24 0.62 NH4TO:.2HIO3
44 • 43 o • 39
76.35 0.31 « +mo3
76 . 70 O HI03
AMMONIUM Per IODATE NH4IO4.
ioo gms. H2O dissolve 2.7 gms. salt at 16°, du = 1.078. (Barker, 1908.)
AMMONIUM IODIDE NH4I.
SOLUBILITY IN WATER. SOLUBILITY IN AQUEOUS ALCOHOL AT 25°.
(Smith and Eastlack, 1916.)
Gms. NHJ
Gms. per ioo Gms. Sat. So
- Solid Phase.
NH,IO3
HIO3.
O
NH4I03.
4-2O
2-54
4-52
6-57
3 '83
1.94
"+NH4IO3.2HIO3
NH4I03.2HI03
Gms.C2H5OH , f
-
(Seidell, unpublished.)
Gms. NH4I per ioo Gms.
— 20
— 10
o
10
15
20
25
30
L iuu \jrui3.
H20.
* .
JC1 IUU VTIIlb.
H20.
PCI iuu vjiiia. <
Solvent.
>at. Sol.
Sat. Sol.
Solvent.
125.2
40
190.5
O 3
[ .646
64.5
l8l.9
136
50
199.6
10 :
C.590
6l.7
161 .1
145
60
208.9
20
•525
58.7
142.1
154.2
70
218.7
30
.462
55-5
124.8
163.2
80
228.8
4°
•395
52
108.3
167.8
IOO
250-3
5° ii
.320
48
92.3
172.3
120
273.6
60
.250
43-8
77-9
176.8
140
299.2
70
.168
39
64
l8l.4
80
.094
33-3
49.9
9°
.013
27-5
37-9
IOO <
5.929
20.8
26.3
53
AMMONIUM IODIDE
Tetra Ethyl AMMONIUM IODIDE N(C2H6)J,
SOLUBILITY IN SEVERAL SOLVENTS.
(Walden — Z. physik. Chem. 55, 698, '06.)
Solvent.
Water
Water
Methyl Alcohol
Methyl Alcohol
Ethyl Alcohol
Ethyl Alcohol
Glycol
Glycol
Acetonitrile
Acetonitrile
Propionitrile
Propionitrile
Benzonitrile
Methyl Sulphocyanide
Ethyl Sulphocyanide
Nitro Methane
Nitro Methane
Nitroso Dimethyline
Acetyl Acetone
Furfurol
Furfurol
Benzaldehyde
Salicylaldehyde
Anisaldehyde
Acetone
Acetone
Ethyl Acetate
Ethyl Nitrate
' Formula.
H20
H2O
CHaOH
CHaOH
C2H5OH
C2H5OH
(CH2OH)2
(CH2OH)2
CHaCN
CH3CN
CH3CH2CN
CH3CH2CN
o
25
o
25
o
25
o
25
o
25
o
25
25
25
25
o
25,
25
CH3COCH2COCH3 25
C4H3O.COH o
C4H3O.COH 25
CeH5COH 25
CeH4.OH.COH 25
CH3SCN
C2H5SCN
CH3NO2
CH3N02
(CH3)2N.NO
C6H4.OCH3.COH
(CH3)2CO
(CH3)2CO
C2H5ONO2
25
o
25
25
25
Benzoyl Ethyl Acetate C6H5COCH2COOC2H5 25
Dimethyl Malonate CH2(COOCH3)2
Methyl Cyan Acetate CH2CNCOOCH3
Methyl Cyan Acetate CH2CNCOOCH3
Ethyl Cyan Acetate CH2CNCOOC2H5
Ethyl Cyan Acetate
Nitrobenzene
Acetophenone
Amyl Alcohol
Paraldehyde
Methyl Formate
CH2CNCOOC2H5
C6H5NO2
25
o
25
o
25
25
Bromobenzene
C5HnOH
(C2H40)3
HCOOCH3
CeHaBr
(Walden
Sp. Gr. Gms. N(C2Ha)4l per IPO.
Solution. cc. Solution. g^
1.0470 16.31 15.58
I.I02I 36.33(35.5) 32.9
0.8326 3-7-4-3 4-44
0.8463 10.5 (10.7) 12.29
0.7928 0.348 0.439
0.7844 0.98(0.88) I.II3
I.I039 3-27 2.97
1.0904 7-63(7.55) 7
0.8163 2.24 2.74;
0.7929 2.97(3.54) 3.74
0.8059 0.618 0.767
0.7830 0.81-1.01 0.99
0.467 0.451
1.0828 4.40 4.06
I. 0012 0.475 0.47
1.1658 '3.59 3-004
1.1476 5.38-6.27 4.72
^.0059 2.67 2.66
0.268
I.I738 3-91 3-33
1.1692 5.33 4.55
0.43
change-
able-i7.7
0.59
0.7991 0.174 0.218
0.249 0.316
.0.00039
1.0984 0.062 0.056
1.1303 0.321 0.284
1.1335 0.040 0.035
1.1341 1.82 1.605
2.83
1.0760 1.057 0.981
1.0607 I-7I 1.41
0.504 0.422
0.13 0.127
0.071 0.089
0.036 0.037
"... 0.031 0.032
'. . . 0.009 0.006
— Z. physik. Chem. 61, 635, igo7-'o8.)
AMMONIUM IODIDE
54
Tetra Methyl AMMONIUM IODIDE N(CH3)4I.
SOLUBILITY IN SEVERAL SOLVENTS.
(Walden — Z. physik. Chem. 55, 708, '06.)
Sp. Gr. of
Cms. N(CH3)4 1
'. per roo.
Solvent.
Formula.
t °.
Solution.
cc
. Solution.
Gms.
Solution.
Water
H20
0
\
.0188
2
.01
I
•97
Water
H20
25
I
•0155
5
•31-5
.89
5
.22
Methyl Alcohol
CH3OH
o
0
.8025
o
.18-0
.22
0
.22
Methyl Alcohol
CH3OH
25
0
.7920
0
.38-0
.42
o
.48
Ethyl Alcohol
C2H5OH
25
0
.7894
o
.09
Glycol
(CH2OH),
0
x
.014
Glycol
(CH2OH)8
25
I
.0678
o
.240
0
.224
Acetonitrfl
CH3CN
25
o
.650
. . .
Nitro Methane
CH3NO,
0
I
•1387
0
.25-0
•32
o
.22
Nitro Methane
CH3NOa
25
I
.1285
o
•34-0
•38
o
.21
Acetone
(CH3)2CO
o
. . .
o
.118
Acetone
(CH3)2CO
25
o
.187
Salicyl Aldehyde
C6H4.OH.COH
0
I
.1492
0
.302
0
.263
Salicyl Aldehyde
CJl4.OH.COH
25
I
•1379
0
.510
o
.484
Very exact determinations of the solubility of tetra methyl ammonium iodide
in aqueous solutions of KOH and of NH4OH at 25° are given by Hill (1917).
Tetra Propyl AMMONIUM IODIDE N(C3H7)4l.
SOLUBILITY IN SEVERAL SOLVENTS,
(Walden — Z. physik. Chem. 55, 709, '06.)
Formula.
CH3OH
CH3OH
C2H5OH
C2H5OH
CHsCN
CHaCN
C2H5CN
Solvent,
Methyl Alcohol
Methyl Alcohol
Ethyl Alcohol
Ethyl Alcohol
Acetonitrile.
Acetonitrile
Propionitrile
Propionitrile
Benzonitrile
Nitro Methane
Nitro Methane
Nitro Benzene
Benzaldehyde
Benzaldehyde
Anisaldehyde
Anisaldehyde
Salicylaldehyde
Ethylnitrite C2H5NO2
Ethylnitrite C2H5NO2
DimethylMalonate CH2(COOCH3)2
DimethylMalonate CH^COOCH^
Acetone (CHs)2CO
Acetone (CH3)2CO '
Ethyl Acetate CH3COOC2H5
Ethyl Bromide C2H5Br
CeH6CN
CH3NO2
CH3NO2
C6H5NO2
C6H5COH
Sp. Gr. of
Gms. N(C3H7)J per 100.
t°.
Solution.
cc. Solution
Gms.
Solution.
0
0.9756
40.92
41.94
25
I.OI87
56.42
55-37
0
0.8349
6.5-6.8
8.14
25
0.8716
19.88-20.29
23-28
0
0.8553
I3-03
15.24
25
0.8584
18.69
21.77
0
0.8280
6.37
7.66
25
0.8191
9-65
10.29
25
I.OI99
8.44
8-35
o
I.lSl
14.79
12.52
25
I.I58
22.24
19.21
25
I-IQ3
5-71
4 79
0
I.058l
7.06
6.67
25
1.0549
9.87
9-35
0
I.III4
5-60
5-04
25
I.I004
6-75
6.14
25
. . .
39.28
o
I.I207
0.522
0.466
25
I.I025
0.653
0.592
o
I-I532
0.298
0.259
25
I-I345
0.320
0.282
0
0.8259
2.692
4-65
25
o . 8049
3-944
4.90
25
0.8975
0.0063
0.007
25
0.187
(Walden — 2. physik. Chem. 61, 639,
55
AMMONIUM IODIDE
SOLUBILITY OF TETRA AMYL, TETRA ETHYL AND TETRA a PROPYL AMMONIUM
IODIDES IN WATER AND IN CHLOROFORM AT 25°. (Peddle and Turner, 1913.)
Gms. Each Salt (Determined Separately), per 100 Gms. Solvent.
Solvent. t * >
N(CsHn)4I. NCCtH^J. aN(C3H7)4I.
Water 0.74 45 18.64
CHC13 210.8 1.55 54.56
Freezing-point data for mixtures of tetra methyl ammonium iodide and iodine,
and for phenyltrimethyl ammonium iodide and iodine are given by Olivari (1908).
AMMONIUM Iridium CHLORIDES.
SOLUBILITY IN WATER AT 19°. (Delepine, 1908.)
Name of Salt. Formula.
^
Ammonium iridium chloride (NH4)2IrCl6 0.77
Diammonium aquo penta chloro indite IrCl5(H2O)(NH4)2 15.4
Triammonium hexa chloro iridite IrCl6(NH4)3+H2O 10.5
AMMONIUM lodo MERCURATE 2NH4I.HgI2.H2O.
100 gms. of the saturated aqueous solution contain 4.5 gms. NH4, 22.6 gms.
Hg and 62.3 gms. I at 26°, sp. gr. = 2.98. (Duboin, 1905.)
AMMONIUM Tetra MOLYBDATE (NH4)2O.4MoO3.2H2O.
100 gms. H2O dissolve 3.52 gms. salt at 15° (d = 1.03), 3.67 gms. at 18° (d =
1.04) and 4.60 gms. at 32° (d = 1.05). (Wempe, 1912.)
AMMONIUM Phospho MOLYBDATE
SOLUBILITY IN WATER AND AQUEOUS SOLUTIONS AT 15°. (de Lucchi, 1910.)
Solvent. Gms. Salt per 1000 Gms. Solvent.
Water 0.238
5 per cent aqueous NHiNOs solution o. 137
i per cent aqueous HNOs solution o . 203
AMMONIUM NITRATE NH4NO3.
SOLUBILITY IN WATER.
(Schwarz — Ostwald's Lehrbuch, ad ed. p. 425; Muller and Kaufmann — Z. physik. Chem,-
42, 497. oi-'oa.)
...
Sp. Gr.
Solution.
G. Mols.
NI^NOa per
loo Mols. HaC
Gms. NH4NO8 per
)ioo Gms.
Solid
Phase.
• Solution.
Water:
0
26
63
54
.19
118
•3
NH4NOa rhomb.
ft
12
2
•2945
34
50
60
•53
153
•4
"
20
2
.3116
43
30
65
.80
192
•4
"
25
O
•3!97
48
19
68
.17
214
.2
M
30
O
•3299
54
40
70
•73
241
.8
ft
32
I
•3344
57
.60
•97
256
•9
NH4NOa rhomb.
ft + rhomb, a
35
.0
•3394
59
.80
72
.64
265
.8
NH4NO8 rhomb.
a
40
o
•3464
66
80
74
.82
297
-0
ii
So
o
77
.41
77
•49
344
• O
M
60
0
94
•73
80
.81
421
.0
M
70
.0
112
•30
83
•32
499
• 0
"
80
.0
130
•5°
85
•25
580
.0
M
90
.0
166
88
.08
740
.0
NH^Oa rhombohedral ?
100
.0
196
oo
89
7i
871
.0
"
SOLUBILITIES OF MIXTURES OF AMMONIUM NITRATE AND OTHER SALTS.
(RUdorf— Mulder.)
loo gms. H2O dissolve 162.9 gms. NH4NO3 + 77.1 gms. NaNO3 at 16° R.
100 gms. H2O dissolve 88.8 gms. NH4NO3 + 40.6 gms. KNO3 at 9° M.
100 gms. H2O dissolve 101.3 gms. NH4NO3 + 6.2 gms. Ba(NO3)2 at 9° M.
AMMONIUM NITRATE
SOLUBILITY OF AMMONIUM NITRATE IN AMMONIA.
(Kuriloff— Z. physic. Chem. 25, 109, '98.)
Gms.
Mols. NEUN03
Gms. per 100 Mols.
Gms.
Mols. NEUNO,
Gms. per 100 Mols,
f.
NEUNOa-
NHa.
+ NHa.
t
o
NH4NO3.
NHa. NH4NO«
+ NHT
80
O
100
0
.0
33
•3
O
•9358
0
2352
45-9
60
1.3918
4-4327
6
•25
35
•9
O
•7746
0
•1857
47 o
44-5
0.9526
1-2457
13
•9
68
.8
4
.2615
o
•7747
53-8
30
0-8308
0.3700
32
•3
94
.0
0
•6439
o
.0665
67-3
10.5
0.9675
o-4&5
36
•9
190
.8
0
•7578
0
.0588
74-2
0
o . 7600
o . 2607
38
•3
168
.0
IOO-O
t° «= temperature of equilibrium between solution and solid phase
SOLUBILITY OF AMMONIUM NITRATE IN AQUEOUS SOLUTIONS OF AMMONIUM
SULFATE AND VlCE VERSA.
(Massinik, 1916, 1917.)
Results
(de Waal
Gms. per
loo Gms. Sat. Sol.
ato°.
, 1910.)
Solid Phase
Results at 30°. Results at 70°.
(Schreinemakers and Haenen, 1910.) (de Waal, 1910.)
Gms. per Gms. per
100 Gms. Sat. Sol. 100 Gms. Sat. Sol.
e~i:j T>I . •• c_i:j T>I — .*_
54-19
(Nl
1 S(
o
[U>2
NH4NO3
70.1
(NH*),
S04.
0
NEUN03
NH4NO3.
84-03
o
J?"
NH4N03
49.12
6
"
67.63
2.38
"
81
-38
2.
4i
"
45-99
9
53
NEUN03+i.3
66.93
3-46
NEUN03+i.3
81
.01
2.
45
NHiNOs+i.s
31.61
19
5
1.3
63-84
4.96
1.3
80
• 25
2.
68
i-3
30.87
20
43
1.3+1.2
58.06
8.22
1.3+1-2
76
.01
3-
96
"
31.04
20,
4
1.2
52.75
11.42
1.2
73
.48
1.3+1.2
29.81
21,
33
"
49.80
13.27
" +(NEU)2S04
.58
5-
82
1.2
29.58
41,
64
i.2+(NEU)2SO4
37.20
19.48
(NH4)2S04
70
• 15
6.
71 3
t.a+(NEWaS04
S.6l
37
89
(NEU)3S04
19.91
28.83
"
ii
.10
40.
81
(NILJzSO,
o
4i
4
"
I2.O5
34-7
"
0
47-
81
"
O
44.1
"
1.2 =
1.3 = (NH4)aS04.3NH,NO..
Freezing-point lowering data for mixtures of ammonium nitrate and lead
nitrate are given by Bogitch (1915).
SOLUBILITY OF AMMONIUM NITRATE IN NITRIC ACID.
(Groschuff — Ber. 37, 1488, '04.)
Determinations by the " Synthetic Method," see Note, page 16.
Gms.
Mols.
Gms.
Mols.
to NH4NOJ
NEUNOa
Solid
t°
NEUNO3
NH4NO3
Solid
Gms.
100
Sol.
per 100
Mols. HNO3.
Phase.
per 100
Gms. Sol.
per 100
Mols. HNO3.
Phase,
8
21
. I
21. 1 ]
tfEUNOa.2HNOa
II.
0
51.7 84 . 3 NH.NO3.HNOs
23
28
•7
31-6
a
12.
0
54.7
95-1
«
labil.
29.5m
Pt. 38
.8
50.O
"
II.
5
57-6
IOS.0
"
b
27
•5
44
.6
63-4
b
II.
5
54-0
92.4 NH4NO3
labil
23
•5
49
• 4
76.8
•'
17.
0
54-7
95-1
stabil
17
• 5
54
.0
92.4
•i
27.
o
56.2
IOI.O
•'
16
4
•5
.0
54
45
:I
93-5
66.7
NEUNO3.HNO3
49-
79-
o
0
60.4
68.1
I2O.O
168.0
••
a =
solution
in HNO8! l
6 =
solution
in NH,NO,.
57
AMMONIUM NITRATE
SOLUBILITY OF AMMONIUM TRI-NITRATE IN WATER.
(Grcschuff.)
Cms. NI^NOs Cms. HNO3 Mols. NH4NO3* Mols. NIL.NO,
per 100 Cms. per 100 Gms. per 100 Mols. per 100 total Solid Phase.
Solution.
Solution.
H20.
Mols. Solution.
O
34-2
53-9
64.3
22
- 2.5
34-8
54-8
75.1
23.1
+ 3
35 4
55-8
90
24-3
8-5
36.6
56-9
"3
25-7
19-5
37-4
58.9
225
29
25
38.1
60
45°
31
29-5
m. pt. 38 8
61.2
00
33
SOLUBILITY OF MIXTURES OF AMMONIUM NITRATE AND SILVER NITRATE IN
WATER AT VARIOUS TEMPERATURES.
(Schreinemakers and deBaat, 1910.)
Gms. per 100 Gms.
to Sat. Sol. Solid Phase. t°.
Gms
. per 100 Gms.
Sat. Sol. Solid Phase.
AgNO3. NI^NOj.
'AgN03.
NH4NO3:
- 7-3
47.
,i
o
Ice+rb
AgNO3
109 6
67
•9
32
.1
D+rb.AgNO3
— 10.7
44-
52
8.43
{
* •
0
22
•13
44
•87
D+rb-NHiNOj
— 14.9
42
16.8
Ice+D+rb
. AgN03
18
27
.07
49
.22
"
-14.8
39
Si
18.79
" +D
30
29
.76
52
•50
"
-18.7
15
99
37-3
" +D+0rb.NH4NO3
±32
{D-frb. NH4NO8+
a+rb. NH4NO3
— 17.4
0
18
30
l/t Cn c/v
OOVx O C
36
:3896
41.2
19-59
22.06
23.42
D+rb.
AgNO3
40
55
85.4
32
36
.68
.6
52
52
.22
.38
D+«rb.NH4NO3
(D+rb.NH4NO3+
\ rbd.NH3NO3
55
63
32
26.12
1
*
101.5
47
• 5
52
• 5
D+rbd. NH3NO3
D = NH4NO3.AgNO3. rb. = rhombic. rbd. = rhombohedric.
SOLUBILITY OF AMMONIUM NITRATE IN AQUEOUS SOLUTIONS OF SILVER
NITRATE AND VICE VERSA AT 30°.
(Schreinemakers and deBaat, 1910.)
Solid Phase.
D
u
D+AgN03
AgN03
Results are also given by Schreinemakers (1908-09) for the reciprocal solubility
of ammonium nitrate and silver nitrate in aqueous alcohol solutions at 30°.
100 cc. anhydrous hydrazine dissolve 78 gms. NH4NO3 at room temp, with
decomp. (Welsh and Broderson, 1915.)
Freezing-point data for mixtures of ammonium nitrate and silver nitrate are
given by Flavitzkii (1909) and by Zawidzki (1904). The eutectic is at 102.4°
and 30.9 Mol. % AgNO3. Results for NH4NO3 + T1NO3 are given by Boks (1902).
Gms. per 100 Gms.
Sat. Sol.
AgN03.
0
NH4N03-
70.1
12.51
21.31
58.64
27-75
29.76
35-62
41.09
54.12
52.5
45-44
39.60
Solid Phase.
Gms. per 100 Gms.
Sat. Sol.
AgNO3.
NH4NO3."
NH4NO3
45-85
34-47
"
52.45
28.86
"
57-93
24-33
"
58.88
23-42
[H4N03+D
63-27
15.62
D
69.08
6-59
Cl
73
o
D = NH4NO3,
,AgN03.
AMMONIUM NITRATE 58
RECIPROCAL SOLUBILITY OF AMMONIUM NITRATE AND SODIUM NITRATE IN
WATER AT o°, 15° AND 30°.
(Fedotieff and Koltunoff, 1914.)
I .
o
0
0
Sol.
•354
.407
.264
' NH4N03.
0
105.5
II8.4
NaN03.
73-33
66
o
i> .
15
15
15
Sol.
1.429
1.405
1.364
' NH4NO3.
155-3
I56.I
159
NaNO3.
75.38
60.76
36.50
15 »
•375
0
83
•9
15
1-350
1 60
27.79
15
.386
24
•03
81
.21
15
I.
330
l62.
3
17.63
•392
42
.81
79
•34
15
I.
298
167.
4
O
15
.401
64.6
78
.06
30
I .
401
0
96.12
15
.417
110
•9
75
.81
30
I.
450
220.
8
88.31
15 1.428
152
75
•35
30
I.
329
232.
6
O
SOLUBILITY
OF AMMONIUM
NITRATE
IN
AQUEOUS ETHYL ALCOHOL.
(Fleckenstein - Physik
. Z.,
6, 419, '05.)
t°
Grams of NH«N03 Dissolved per 100 Grams Aq. Alcohol of (Wt. %):
100%.
86.77%.
76.12%.
51.65%.
25.81%.
0%.
20 2.5
II
23
70
I4O
195
30 4
14
32
90
165
230
40 5
18
43
196
277
50 6
24
55
144
244
365
60. 7.5
30
70
183
320
70 9
41
93
230
80 10.5
56
NOTE. — The figures in the preceding table were read from curves shown in
the abridged report of the work, and are, therefore, only approximately correct.
Determinations of the solubility in methyl alcohol solutions were also made but
not quoted in the abstract. The "Synthetic Method" (see Note, page 16) was
used.
100 grams absolute ethyl alcohol dissolve 4.6 grams NKUNOs at 14° and 3.8
100 grams absolute methyl alcohol dissolve 14.6 grams NP^NOs at 14°, 16.3
grams at 18.5° and 17.1 grams at 20.5°.
(Schiff and Monsacchi — Z. physik. Chem., 21, 277, '96; at 20.5° de Bruyn — Ibid., 10, 783, '92.)
SOLUBILITY OF AMMONIUM NITRATE IN AQUEOUS ETHYL AND METHYL
ALCOHOLS AND IN A MIXTURE OF THE Two AT 30°.
(Schreinemakers, 1908-09.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
H20.
QHsOH.
NILJSTOa.
H20.
CH3OH.
NIL.NO3.
H20.
*CH3OH
+Q.H.O.
NH<NO.
0
96
•4
3-6
0
83.3
16
•7
3-4
•9
II.7
5
89
.6
6.5
5
74-8
21
•3
5
82
•9
12.3
10
80
•4
10.7
10
63-8
27
.1
10
74
.6
16.4
15
68
.6
17
15
50.7
35
15
63
•5
24
20
53
•5
26.8
20
35-2
46
•3
20
48
.2
35.1
25
32
•5
44-8.
25
19.8
59
25
22
•4
54
29.9
0
70.1
29.9
0
70
.1
29.9
0
70.1
• Weight per cent CH3OH = si-7, C2H5OH = 48.3.
Additional determinations of the solubility of ammonium nitrate in aqueous
ethyl alcohol solutions at o°, 30° and 70° are given by deWaal (1910). At cer-
tain concentrations at 67.5° the solutions separate into two layers.
59
AMMONIUM NITRATE
AMMONIUM Magnesium NITRATE 2NH4NO3.Mg(NO3)2.
100 parts water dissolve 10 parts salt at 12.5°.
(Foucroy.)
AMMONIUM Manganic MOLYBDATE 5(NH4)2MoO4.Mn2(Mo2O7)s.i2H2O.
100 parts water dissolve 0.98 part salt at 17°. (Struve — J. pr. Chem., 6i,'46o, '54.)
AMMONIUM OLEATE Ci7H33COONH4.
SOLUBILITY IN SEVERAL SOLVENTS.
(Falciola, 1910.)
Solvent Cms. QiHssCOONIL, dissolved per 100 cc. solvent:
Absolute Alcohol 31 at o° 59 at 10° 100 at 50°
75 per cent Alcohol ... 8.2 at. 20° 10 . 86 at 30°
i part Alcohol + 2 parts Ether ... 9.45 at 15° 16.9 at 20°
Acetone ... 4.7 at 15°
AMMONIUM OXALATE (COONH4)2.H2O.
SOLUBILITY IN WATER.
(Av. curve from results ot Engel, 1888; Foote and Andrew, 1905; Woudstra, 1912; Colani, 1916.)
O
IO
15
20
Cms. (COONH4)2 per
100 Gms. Sat. Solution.
2.1
3
3-5
4.2
25
30
40
Gms. (COONH4)2 per
100 Gms. Sat. Solution.
4.8
5-6
7-4
9-3
SOLUBILITY IN AQUEOUS SOLUTIONS OF OXALIC ACID.
(Woudstra, 1912.)
Results at 30°. (Interpolated
from Original.)
(COONHi)2.
(COOH),.
ooiiu .rua.se.
(COONH4)2.
(COOH)2.
DOIIQ rnase.
0.14
12.36
A
O.22
21 .22
A
0.28
12.78
A+T
0.31
21.31
(i
0.30
12
T
o-53
20.54
A+T
0-39
10
a
0.56
21.23
T
0.47
8
((
0.61
20-55
u
0.52
7
it
0-54
20.92
tt
0.68
6
tt
0.79
16.44
tt
i
5
(C
1.23
12.88
tt
2
3-96
(I
7.16
7.98
tt
3
3-6i
((
3-54
5-83
tt
4
3-6o
u
5-65
5-67
it
5
3.81
((
6.72
5-95
tt
5-98
4.21
T+A. O.
8.74
6-53
T+A. O.
7
3-63
A. O.
8-93
6.27
A. O.
8.19
3-36
A. O.+N. O.
9.04
6.14
u
7
2.32
N. O.
12.38
5
A. O.+N. O.
6
1.02
a
8.31
3-°4
N. O.
5-53
O.22
u
9-59
i-45
tt
A. = Oxalic Acid (COOH)2.H2O.
A. O. = Acid Ammonium Oxalate (COO)2HNH4.H2O.
T = Ammonium tetroxalate (COOH)2(COO)2HNH4.2H2O.
N. O. = Neutral Ammonium Oxalate (COONH4)2.H2O.
Additional data for this system at 25° are given by Walden (1905), and at o°,
by Engel (1888).
AMMONIUM OXALATE
60
SOLUBILITY IN WATER OF MIXTURES OF AMMONIUM OXALATE AND:
Other Oxalates at 25°.
(Foote and Andrew, 1905.)
Cms. per 100 Cms. Sat. Solution.
2.79 (COONH4)2.H20 + 2 5 . 96 (COOK)2H2O 1 5
4.8 " +5-75 (COOLi)2 50
5.45 " +0.59 (COO)2Mg.2H20 18
6.19 " +1.45 (COO)2Zn.2H2O 50
5 . 06 " +o . 28 (coo)2 Cd.3H2o 19
50
Other Ammonium Salts.
(Colani, 1916.)
Gms. per 100 Gms. Sat. Solution.
0.14 (COONH4)2 + 26.35 NH4C1
0.67
O.II
0.65
0.085
o-35
+32-55
+42.43 (NH4)2S04
+45-92 "
+ 62.26 NH4N03
+ 72.11
Both salts in excess in every case. No double salts formed.
SOLUBILITY OF AMMONIUM OXALATE AND OF AMMONIUM THORIUM OXALATE
IN WATER AT 25°.
(James, Whittemore and Holden, 1914.)
The mixtures were constantly agitated for periods varying from many weeks
to several months.
Solid Phase.
2.I.7+2.I.2
2.1.2
(t
2.1.2 = 2Th(C2O4)2.(NH4)2C2O4.2H2O.
gms. (NH4)2C2O4 at 21°. (Aschan, 1913.)
44 gms. (NH4)2C2O4 at room temp.
(Welsh and Broderson, 1915.)
Gms. per 100 Gms. H2O.
Solid Phase.
(NHdtCA.
Th(C2O4)2.
5-25
0 (1
srH4)2c2<
L/4
6.04
i-54
tt
7-78
4-51
a
10.37
8.87
(f
15.46
16.89
((
21.47
26.37
tt
28.18
36.54
"+2,
•i-7
Gms. per 100 Gms. H2O.
(NH4)2C204.
29.47
23.04
16.84
Th(C204)2.
39-iQ
29-87
21. l8
13.27
8.13
5.36
15.96
9-13
5-63
1.70
1.42
2.1.7 = 2Th(C204)2.(NH4)2C204.7H20;
100 gms. 95% formic acid dissolve 6.2
100 cc. anhydrous hydrazine dissolve
with evolution of ammonia.
AMMONIUM PALMITATE Ci6H3iO2NH4.
SOLUBILITY IN SEVERAL SOLVENTS.
(Falciola, 1910.)
Gms. Ci6H31O2NH4 per 100 c.c. of:
«••
Absolute
Alcohol.
75% Alcohol.
50% Alcohol.
Mixture of i Pt.
Alcohol + 2 Parts
Ether.
Acetone.
0
10
o-5
0.7
I. '78
0.37(13°)
0.2 '(13°)
20
1.4
4-33
5-33
O.29
30
40
4-5
EI.02
14.84
6.69
50
ii
. . •
AMMONIUM PHOSPHATES (NH4)3PO4, (NH4)2HPO4, and NH4H2PO<.
loo gms. H2O dissolve 131 gms. (NH4)2HPO4 at 15°, du sat. sol. = 1.343.
(Greenish and Smith, 1901.)
Data for the solubility of mono ammonium phosphate in anhydrous and in
aqueous ortho phosphoric acid, determined by the synthetic method, are given
by Parravano and Mieli, 1908.
6i AMMONIUM PHOSPHATES
SOLUBILITY OF
Cms. per 100 Gms.
Sat. Solution.
AMMONIUM PHOSPHATES IN AQUEOUS SOLUTIONS OF £)RTHO
PHOSPHORIC ACID AT 25°.
(Parker, 1914.)
Gms. per 100 Gms.
Solid Phase. Sat- S9lution. Solid Phase.
H3PO4. NH3.
4.1 22.6
4-4 18.4
10 13.1
20 7
30 7-7
34.4 10
40 10.2
48 . 2 ii .6
(NH4)3P04.3H20
It
tt
11
(NH4)3P04.3H20+ (NH4)2HP04
(NH4)2HPO4
(NH4)2HP04+NH4H2PO4
H3P04. NH3.
40 9
30 5-4
20.6 4
30 3-8
40 4
50 4.2
60.6 4.4
tfH4H2P(
n
n
ti
tt
tt
tt
The original figures have been calculated to grams, plotted on cross-section
paper and the above table read from the curve.
Data for this system are also given by D'Ans and Schreiner (1910). The
agreement is satisfactory except for the (NH^aPO^HaO end of the curve, for which
much lower values for the NHs component are given by D'Ans and Schreiner.
AMMONIUM Magnesium PHOSPHATE NH4MgPO4.6H2O and iH,O.
SOLUBILITY IN WATER AND SALT SOLUTIONS,
(Bube, 1910.)
The solutions were saturated in 7-16 liter flasks. The stirrer was introduced
through a mercury sealed connection, in order to prevent loss of moisture or
ammonia during the long periods required for saturation, ^reat care was ex-
ercised to eliminate errors of manipulation. Large volumes of the saturated
solutions were used for analysis. In the cases where equilibrium was approached
from above (designated by *, in table below) the mixtures were heated to about
90° for \ hour, and then cooled while being continually stirred for 4-5 hours at
50°, and then in a thermostat at 25° for the remaining period shown.
Solver t° Time for Cms, per 100 Cms. Sat. Sol.
* ' Saturation. ^7 p^ NH^
Water 25° 69 hrs. 0.0808 0.0965 ... Mixed Hydrates
" 25 9 days 0.0867 0.0992
25 14 " 0.1352 0.1333 0.1301
" 22.7 17 hrs.* 0.1076 0.1084. 0.1040 Monohydrate
anNI^Cl 25 20 days 0.3129 0.3057 ... Mixed Hydrates
— »NH4Cl+i»NHs 25.2 16 hrs.* 0.0249 0.02025 ... Monohydrate
0.2 Mol. MgCl2 per liter H2O 25 27 days ... 0.0206 ... Mixed Hydrates
0.2 " " " " 25.2 16 hrs.* ... 0.0512 ... Monohydrate
-i- Mol. (NH4)2HPO4 per liter H2O 24 . 25 ... * 0 . 1 229 ... ... "
3*2
SOLUBILITY OF AMMONIUM MAGNESIUM PHOSPHATE IN SEVERAL SOLVENTS.
(Wenger, 1911.)
Cms. NH4MgPO< per 100 Cms. Solvent in:
t°.
Water.
Aq. 5%
AqwSn°
Mixture of i Pt.
NH3(<f=o.96)
NH.ci+4
Aq. 10%
NH4Cl+4
NH4NO3.
NH4C1.
+4 Pts. H2O.
NH3 per 100.
NH3 per 100.
0
0.023
O.IIO
0.060
0.0087
. . .
. . .
20
O.O52
0.046
0.105
0.0098
0.0l65
0.0541
30
. . .
0.054
O.II3
.
40
0.036
0.064
0.071
O.OI36
50
O.O3O
O.O72
0.093
0.0153
60
0.040
0.085
0.173
0.0174
0.0274
0.0731
70
0.016
0.083
O.I24
0.0178
...
80.
0.019
O.IOI
O.I9I
0.0145
...
...
AMMONIUM PHOSPHATES
62
AMMONIUM
Manganese PHOSPHATE NH4MnPO4.7H,O.
SOLUBILITY IN SEVERAL SOLVENTS.
(Wenger, 1911.)
Gms. NH^MnPC^ per 100 Gms. Solvent in:
Water.
KH^NO".
0.021
Aq. 5%
NH4C1.
O.OO2
Mixture of i Pt. NH3
(d =0.96) +4 parts H2O.
0.0116
0
0.020
0.025
0.0122
0
0.023
O.O2I
0.034
0.039
o.onS
O
0.005
0.023
0.027
O.O28
0-035
0.038
O.O4I
0.0132
0.0194
0.0191
0.007
0.033
0.045
0.0197
O
20
30
40
50
60
70
80
AMMONIUM Sodium PHOSPHATES
Data for the distribution of each of 5 ammonium sodium ortho- and pyro-
phosphates between water and chloroform at 18°, are given by Abbott and Bray
(1909).
AMMONIUM Hydrogen PHOSPHITE (NH4H)HPO3.
100 grams water dissolve 171 grams (NH4H)HPO3 at o°, 190 grams at 14.5°
and 260 grams at 31°. (Amat., 1887.)
AMMONIUM Hypo PHOSPHITE NH4H2PO2.
100 cc. H2O dissolve 83 gms. NH4H2PO2 at room temp.
(Squire and Caines, 1905.)
AMMONIUM PERMANGANATE NH4MnO4.
100 parts water dissolve approximately 8 parts of NH4MnO4 at 15°. (Aschoff.)
AMMONIUM PICRATE C6H2(NO2)3ONH4.
100 cc. H2O dissolve i.i gm. Am. picrate at room temp. (Squire and Caines, 1905.)
100 cc. 90% alcohol dissolve 1.2 gm. Am. picrate at room temp.
(Squire and Caines, 1905.)
AMMONIUM Fluo SILICATE (NH4)2SiF6.
100 parts water dissolve 18.5 parts (NH4)2SiF6 at 17.5,° Sp. Gr. 1.096.
(Stolba, 1877.)
AMMONIUM SALICYLATE C6H4.OH.COONH4.
SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1909, 1910.)
Gms. C2H6OH s
per too Gms.
Solvent.
3. Gr. of
at. Sol. x
Gms. C6H4.
OHCOONH4 per
oo Gms. Sat. Sol.
Gms. C2H5OH
per 100 Gms.
Sat. Sol.
Sp. Gr. of c
Sat. Sol.
Gms. C6H4.OH.
:OONH4 per too
Gms. Sat. Sol.
0
.148
50.8
70
I.OI5
42
20
.122
50.3
80
0.979
38
40
.088
48.3
90
0.936
31.6
50
.067
46.7
95
0.907
27.8
60
.042
44-7
•100
0.875
22.3
AMMONIUM SELENATE (NH4)2 SeO4
loo gms. H2O dissolve 1.22 gms. (NH4)2 SeO4 at 12°.
(Tutton, 1907)
63
AMMONIUM STEARATE
Absolute Alcohol. 75% Alcohol. 50% Alcohol.
AMMONIUM STEARATE Ci8H36O2NH4.
SOLUBILITY IN SEVERAL SOLVENTS.
(Falciola, 1910.)
Cms. CigHjaANIL, per 100 cc. of:
O
10
20
30
40
50
O.I
0.9
1.8
5-5
0.56
1.83
5
0.25
1.16
3-21
Ether.
O.I
Acetone.
0.08 fo
AMMONIUM SULFATE (NH4)2SO4.
SOLUBILITY IN WATER.
(Mulder.)
Grams (NBU)2SC>4 per 100 Grams.
O
5
10
15
20
25
Water.
70.6
71.8
73-o
74-2
75-4
76.7
Solution.
41.4
41.8
42 .2
42.6
43-o
43-4
t°.
Grams (NIL^S
D4 per TOO G
' Water.
Solution o
30
78.0
43-8
40
81.0
44.8
60
88.0
46.8
80
95-3
48.8
100
103 .3
50 8
108.9
I07-5
5i-8
Sp. Gr. of saturated solution at 15° — i 248; at 19° = 1.241
Eutectic point, Ice + (NH4)2SO4 = — 19.05° and 38.4 gms. (NH4)2SO4 per 100
gms. sat. solution.
SOLUBILITY IN AQUEOUS AMMONIA SOLUTIONS AT 25°.
(D'Ans and Schreiner, 1910.)
Mols. per 1000 Gms. Sat. Sol.
Gms. per looo^Gms. Sat. Sol.
(NHa).
(NH4)2S04.
0
3-28
I .02
2.60,
i-95
2.13
3-44
i-S9
5-35
i .16
7-i3
0.78
9-47
0
'(NH3).
(NH4)2S04.
O
433-4
17.4
343-6
33-2
281.5
58.6
210. 1
91.1
153-3
121.4
103
161.2
0
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS SOLUTIONS OF COPPER
SULFATE AT 30° AND VICE VERSA.
(Schreinemakers, 1910.)
Gms. per 100 Gms. Sat.
Solution.
CuS04.
o
Solid Phase.
Gms. per 100 Gms. Sat.
Solution.
Solid Phase.
44
38.32
29.27
17.53
9.33
(NH4)2SO4
8.19
1. 1. 6
1. 1.6
CuSO4.
13.65
16.77
20.53 i.i.6-fCuSO4.5H2O
20.19 CuSO4.5H2O
° 20.32
* = Solubility of 1.1.6 in water.
1. 1.6 = CuSO4(NH4)2SO4.6H2O.
Several additional determinations for the above system at 19°, are given by
Riidorff (1873), and by Schiff (1859).
0.77
1.57
4-°S
11.03
(NH4)2S04+i.i.6 6.98
5.79
2.45
AMMONIUM SULFATE
64
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS SOLUTIONS OF FERROUS
SULFATE AT 30° AND VICE VERSA.
(Schreinemakers, 1910 a.)
Gms.
per 100 Gi
Solution.
T1S.
Sat.
Solid Phase.
(NH4)2S04
(NH)SO+i.i.6
1. 1.6
it
u
Gms. per 100 Gms
Solution.
.Sat.
Solid Phase.
1. 1.6
it
i.i.6+FeSO4.7H2O
FeSO4.7H20
(NH4)2S04.
'44.27
43-88
34.24
19.64
16.29
n-45
FeS04.
O
o-79
1.72
5-70
7-95
(NH4)2S04.
8.90
6.44
5-91
5-24
O
FeS04. '
17.64
23-59
25.24
25.24
24.90'
1.1.6 = (NH4)2SO4.FeSO4.6H2O.
Data for the quaternary system (NH4)2SO4o + FeSO4 + Li2SO4 + H2O at 30°
are. also given.
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS SOLUTIONS OF LITHIUM
SULFATE AND VICE VERSA.
(Schreinemakers, Cocheret, Filippo and deWaal, igos^igo;.)
Results at 30°.
Results at 50°.
Gms. per 100 Gms. Sat.
Solution.
Solid Phase.
Gms. per 100 Gms. Sat.
Solution.
Solid Phase.
(NH4)2S04.
Li2S04-
(NH4)2S04.
Li2S04.
44
.1
0
(NHJjSO*
45
•7
0
(NIL^SO,
40
.8
3
43
•05
5.86
(NH4)2SO4+NH4LiSO4
39
•5
6.6
(NH4)2SO4+NH4LiSO4
19
•65
16.35
NH4LiSO4
30
10
NH4LiSO4
13
.90
21.20
"
21
.6
15
«
13
•97
21.23
NH4LiS04+Li2S04.H2O
15
20
«
ii
•45
21-75
Li2SO4.H2O
12
-5
21.9
NH4LiSO4+Li2SO4.H2O
9
•63
22.79
"
8
•9
23
Li2SO4.H2O
8
•58
23.09
«
0
25.1
"
7
•56
22.86
«
o
24-3
"
Additional data for the triple points of the above system at 20°, 57° and 97°
are given by Spielrein (1913), but the terms in which the results are presented
are not clearly shown.
Data for the quaternary system, ammonium sulfate, lithium sulfate, alco'hol
and water at 6.5°, 30° and 50° are given by Schreinemakers and van Dorp (1907).
A mixture of an excess of ammonium and of potassium sulfates in water at
19° was found by Rudorff (1873) to contain 37.97 gms.^ (NH4)2SO4 + 39-3 gms.
K2SO4 per 100 gms. sat. solution.
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 30°.
(Van Dorp, 1910 and 1911.)
Gms. per 100 Gms. Sat.
Solution.
(NH4)2S04. *
H2S04.
44-3
43-6
O
10
44.1
13.2
42.9
15
41
40.8
20
25
43
45-5
30
33-8
42.3
35
Solid Phase.
(NH4)2S04
(NH4)2S04+3.i
3.i+(NH4)HS04
(NH4)HSO4
3.i=3[(NH4)2S04].H2SO.
Gms. per 100 Gms. Sat.
Solution.
(NH4)2S04.
H2S04.
32-8
40
26.1
45
20.9
50
I7.6
55
I7.8
60
20
61.7
30
62.9
37
62.2
Solid Phase.
(NHOHSO
6s AMMONIUM SULFATE
Data for the solubility of ammonium sulfate in aqueous solutions of sulfuric
acid of concentration extending to 10 gm. mols. per liter, are given by D'Ans
(1909 and 1913).
Data for the solubility of ammonium and lithium sulfates in concentrated
sun uric acid containing traces of water, at 30°, are given by Van Dorp (1913-14).
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS SOLUTION OF ETHYL
ALCOHOL AT 30° AND AT 50°.
(Results at 30°, Wibaut, 1909; at 50°, Schreinemakers and.de Baat, 1907.)
Results at 30°. Two liquid layers are formed at concentrations of alcohol
between 5.8 and 62%. These have the compositions:
Upper Layer. Lower Layer.
Gms. per 100 Gms. Sat Solution. Gms. per 100 Gms. Sat. Solution.
(NH4)2SO4. C2H8OH. H2O. (NH»)jSO4. QHBOH. H2O.
2.2 56.6 41.2 37.1 5.8 57.1
2.6 54.5 42.9 35.7 6.3 58
3-4 52-3 44-3 33-8 7-4 $8-8
13.2 31.8 55. 21.7 18.4 59.9
17 25 58 17 25 58
At a concentration of 62% alcohol the liquid is homogeneous and contains
1.3 gms. (NH4)2SO4 per 100 gms. sat. solution, At 90.4% alcohol no (NH4)2SO4
is dissolved.
Results at 50°.
Gms. per too Gms. Saturated Solution.
43.02 2.32 ' 54.66
41.1 4-1 54-8
1-2 64.5 34.3
0-2 75.5 24.3
Between the concentrations 4.1 and 64.5% C2H5OH the mixtures separate
into two layers. The percentage composition of each member of several such
conjoined layers, is as follows:
Upper Layer. Lower Layer.
Gms. per 100 Gms. Sat. Solution. Gms. per roo Gms. Sat. Solution.
(NH4)2SO4. QHSOH. H2O. (NHt)iSO4. QHsOH. H2O.
1.2 64.5 34.3 4I.I 4.1 54.8
1.6 60 38.4 36.8 6 57.2
3.8 50 46.2 30.8 9 60.2
7.4 40 52.6 26.6 12 61.4
10 34.4 55.6 23.6 15 61.4
Two determinations at o° Jby deWaal (1910) gave 30 gms. (NH4)2SO4 per 100
gms. sat. solution in 9.41% alcohol and 0.14 gm. (NH4)2SO4 in 73.03% alcohol.
Between these concentrations of alcohol two liquid layers are formed.
loo gms. 95% formic acid dissolve 25.4 gms. (NH4)2SO4 at 16.5°.
(Aschan, 1913.)
AMMONIUM SULFATE 66
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS ETHYL ALCOHOL SOLUTIONS.
(Continued.)
(Traube and Neuberg — Z physik. Chem. i, 510, '87; Bodlander — Ibid. 7, 318, '91; Schreinemaker —
Ibid. 23, 657, '97 ; de Bruyn — Ibid. 32, 68, 'oo; Linebarger — Am. Ch. J. 14, 380, '"92.)
Upper Layer Results.
Grams per 100 Gms. Solu-
tion at io°-4o°.
Lower Layer Results.
Gms. C8H5OH Gms. (NH<)2SO4 per 100 g.
per 100 Gms. Solution at:
CaHeOH.
(NH4)2S04.
Solution.
6.5°.
IS0-
33°.
100
O-O
O
42 .O
42.6
44
80
o.-i
2-5
39-o
40.2
?
70
o-3
36.2
37-2
?
60
1.4
7-5
33-2
34-5
42
50
3-2
IO-O
30.0
31.0
35
45
4.8
12.5
27.2
28.0
40
6.6
15-0
24.6
25.2
?
35
9.2
'75
22 .O
22.4
?
30
12.2
20-0
20.0
20. o
?
25
14.6
NOTE. — When ammonium sulfate is added to aqueous solutions of alcohol,
it is found that for certain concentrations and temperatures the solutions sep-
arate into two liquid layers, the upper of which contains the larger percentage
of alcohol.
Most of the determinations which have been made upon this system, as con-
tained in the papers referred to above, are given in terms of grams of ammo-
nium sulfate, of alcohol and of water per 100 grams of these three components
taken together. Those results which are given in other terms can be readily
calculated to this basis, and it is, therefore, possible to make a comparison of the
several sets of determinations by plotting on cross-section paper and drawing
curves through the points. In the present case the grams of alcohol per 100
grams of solution were taken as ordinates, and the grams of ammonium sulfate
in the same quantity of each solution taken as abscissae. It was found that a
single curve could be drawn through practically all the points representing the
upper layer solutions at the several temperatures, but the points for the solutions
containing the larger amounts of water gave curves which diverged with increase
of temperature. The results given for 33° in the above table are not to
be accepted as correct until further work has been done.
SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS PROPYL ALCOHOL SOLUTIONS
AT 20°.
(Linebarger — Am. Ch. J. 14, 380, '92.)
Gms per 100 Gms,
Gms. per
100 Gms.
Solution.
Solution .
CaH7OH.
(NH4)2SO4.
C3H7OH.
(NH4)2SO4c
70
0-4
40
3-2
60
1.0
30
4.8
50
2.0
20
6.7
67 AMMONIUM Cadmium SULFATE
AMMONIUM Cadmium SULFATE (NH4)2Cd(SO4)26H2O.
100 cc. H2O dissolve 72.3 gms. (NH4)2Cd(SO4)2 at 25°. (Locke, 1901.)
AMMONIUM Chromium SULFATE (Alum) (NH4)2Cr2(SO4)4.24H2O.
100 cc. H2O dissolve 10.78 gms. anhydrous or 21.21 gms. hydrated salt at 25°.
(Locke, 1901.)
AMMONIUM Cobalt SULFATE (NH4)2Co(SO4)2.6H2O.
SOLUBILITY IN WATER.
(Tobler — Liebig's AnnalenQS, 193, '55; v. Hauer— J. pr. Chem. 74, 433. '58; at 25°, Locke— Am
Ch. J. 27, 459. V>i.)
Gms. (>
rH4)2Co(S04)2 Gms. (NH4)2Co(SO4)2
t°. Per
ioo Gms.
t°.
per
ioo Gms.
Water.
Solution.
'Water.
Solution.'
0 .6.0
5-7
40
22 -O
18.0
10 9.5
8.7
50
27.0
21-3
2O I3-O
"•5
60
33-5
25.1
25 14.72
12.8
70
40.0
28.6
30 17.0
14-5
80
49-o
32-9
NOTE. — The determinations reported by the above named inves-
tigators were plotted on cross-section paper and although considerable
variations were noted, an average curve which probably represents
very nearly the true conditions was drawn through them, and the above
table made from this curve.
AMMONIUM Indium SULFATE (NH4)2In2(SO4)4.24H2O.
ioo gms. H2O dissolve 200 gms. salt at 16° and 400 gms. at 30°. (Rossler, 1873-)
AMMONIUM Iron SULFATE (Alum) (NH4)2Fe2(SO4)4.24H2O.
ioo cc. H2O dissolve 44
25°. Sp. gr. of saturated j
ioo cc. H2O dissolve 44.15 gms. anhydrous or 124.40 gms. hydrated salt at
solution at 15° = 1.203. (Locke, 1901.)
AMMONIUM Iron SULFATE (ferrous) (NH4)2Fe(SO4)2.6H2O.
SOLUBILITY IN WATER.
(Tobler; at 25°, Locke — Am. Ch. J. 2KK, 459, '01.)
0
G. (NH4)2Fe(S04)2
0
G. (NH4)2Fe(SO4)2
0
G, (NH4)2Fe(S04)2
*
per ioo g. H2O.
per ioo g. H2O.
per ioo g. H2O.
o
12 5
25
25.o(T)
50
40
15
20-0
25
35-i(L)
70
52
40
33 o
AMMONIUM Lead SULFATE (NH4)2SO4.PbSO4.
SOLUBILITY IN WATER.
(Barre, 1909.)
Gms. (NH4)2SO4 per ioo Gms.
Sat. Solution.
Water.
20
12.17
13.86
50
16.15
19.25
75
19.52
24.31
IOO
22.74
29.42
(NH4)2SO4.PbSO4
AMMONIUM Lithium SULFATE 68
AMMONIUM Lithium SULFATE NH4LiSO4.
SOLUBILITY IN WATER.
(Schreinemakers, Cocheret, Filippo and deWaal, 1905, 1907.;
Cms. NH4LiSO4 Cms. NH4LiSO4
t°. per 100 Cms. Solid Phase. t°. per 100 Gms. Solid Phase.
Sat. Sol. Sat. Sol.
o o Ice -10 35.25 NKjLiSC^
- 5 14 +10 35-58
-io 23.5 30 ^.87
-15 29.7 50 36
-2o.6Eutec. 35.15 Ice+NH4LiSO4 70 36.18
AMMONIUM Magnesium SULFATE (NH4)2Mg(SO4)2.
SOLUBILITY OF AMMONIUM MAGNESIUM SULFATE IN WATER.
(Porlezza, 1914.)
to. Gms per xoo Gms. ^ ^ ^ Cms. per .zoo Gms.
Sat. Sol. Water. Sat. Sol. Water.
—0.34 1. 01 1.02 Ice 20 15.23 17.96 (NH4)2Mg(SO4)a
—0.8o 2.98 3.07 25 16.45 19-69
-1.23 4.92 5.17 30 17.84 21.71
— 1. 60 6.56 7-02 40 20.51 25.86
— 2.02 8.34 9.10 " 50 23.18 30.17
-2.34Eutec lce+(NH4)2Mg(S04)2 60 26.02 35.17
O 10.58 11.83 (NILJMgSO, 80 32.58 48.32
io 12.75 14.61 " loo 39.66 65.72 "
AMMONIUM Manganese SULFATE (NH4)2Mn(S04)2.6H2O.
100 cc. water dissolve 37.2 gms. (NH4)2Mn(SO4)2 at 25°. (Locke, 1901.)
AMMONIUM Nickel SULFATE (NH4)2Ni(SO4)2.6H2O.
SOLUBILITY IN WATER.
(Average curve from Tobler, Locke, at 25°.)
G. (NH4)2Ni(S04)2
G. (NH4)2Ni(S04)2
t°.
per
ioo Gms.
t°.
per
ioo Gms.
Water.
Solution.
Water.
Solution.
0
1.0
0-99
40
12 .O
IO.72
10
4.0
3-85
50
14-5
12.96
20
6-5
6.10
60
17-0
14-53
25
7-57
7.04
70
20. o
16.66
30
9.0
8-45
AMMONIUM Sodium SULFATE NH4NaSO4.2H2O.
ioo gms. water dissolve 46.6 gms. NH4.NaSO4.2H2O at 15° Sp. Gr., of Sol.
1.1749.
AMMONIUM Strontium SULFATE (NH4)2SO4.SrSO4.
SOLUBILITY IN WATER.
(Barre, 1909.)
t°. Gms.^Hj.SO.perxooGms. Solid Phase.
Sat. Solution. Water.
50 <43-99 78.54
75 45-40 83.15
ioo 46.27 66.2
69 AMMONIUM Vanadium SULFATE
AMMONIUM Vanadium SULFATE (Alum) (NH4)2V2(SO4)424H2O.
100 cc. H2O dissolve 31.69 gms. anhydrous or 78.50 gms. hydrated salt at 25°.
AMMONIUM Zinc SULFATE (NH4)2Zn(SO4)2.6H2O.
SOLUBILITY IN WATER.
(Average curve, see NOTE, p. 67, Tobler, Locke, at 25°.)
G. (NHJzZntSO^a G. (NIL^ZnCSOJj
^•f per 100 Gms. $o^ per 100 Gms.
Solution. Water. Solution. Water.
o 6.54 7.0 40 16.66 20
10 8.67 9.5 50 20.0 25
20 II. II 12-5 6b 23.1 30
25 12.36 14.1 70 25.9 35
30 13-79 16.0 80 29.6 42
AMMONIUM PERSULFATE (NH^S-A.
100 parts H2O dissolve 58.2 parts (NHOsSgOg at o°. (Marshall, 1891.7
AMMONIUM Sodium Hydrogen SULFITE (NH4)Na2H(SO3)24H2O.
100 gms. H2O dissolve 42.3 gms. salt at 12.4° and 48.5° gms. at 15°.
(Schwincker, 1889.)
AMMONIUM Antimony SULFIDE (Sulfoantimonate) (NH4)3SbS4.4H2O.
SOLUBILITY IN WATER AND IN AQUEOUS ALCOHOL.
(Donk, 1908.)
In Water. In Aqueous Alcohol at 10°.
,„ Gms. (NH4)3SbS4 c: IM Pll!10, Gms. per 100 Gms. Sat. Solution.
per 100 Gms. Sat. Sol. ' C2H6OH. (NH^SbS.. "
— 1.9 9.9 Ice o 43.2
- 5 20 5-i 35-9
- 8 30.2 19.1 23.1
-13.5 41-6 Ice+(NH4)3SbS4.4H2O 43.1 8.7
o 41.6 (NH4)3SbS4.4H2O 53.1 4.1
+ 20 47-7 93-3 o
30 54-5
AMMONIUM 0-Naphthalene Mono SULFONATE Ci0Hi7SO3NH4.
100 cc. of the saturated aqueous solution contain 13.05 gms. of the salt at
25°, and dz$ = 1.034. (witt» I9I5->
AMMONIUM Phenanthrene Mono SULFONATES Ci4H9SO3NH4 (2), (3) and
SOLUBILITY IN WATER AT 20°.
(Sandquist, 1912.)
ioo gms. H2O dissolve 0.37 gms. Ci4H9SO3NH4 (2).
100 gms. H2O dissolve 0.26 gms. d4H9SO3NH4 (3).
ioo gms. H2O dissolve 4.41 gms. Ci4H9SO3NH4 (10).
AMMONIUM 2.5 di-iodobenzene SULFONATE C6H3I2SO3(NH4).
ioo gms. H2O dissolve 4.35 gms. salt at 20°. (Boyle, 1909.)
AMMONiUM TARTRATES (NH4)2C4H4O6.
ioo cc. H2O dissolve 2.83 gms. (NH4)2C4H4O6.2H2O at o°. (Fenton, 1898.)
ioo cc. H2O dissolve 5.9 gms. (NH4)2C4H4O6 at 15° (d = 1.04).
(Greenish and Smith, 1903.)
AMMONIUM Lithium TARTRATES dextro and racemic.
ioo gms. sat. sol. inH2O contain 13. 104 gms. racemate(NH4)Li(C4H4O6).H2Oat2O°.
ioo gms. sat. solution in H2O contain 14.186 gms. dextro (NH4)Li(C4H4O6).
£ H2O at 20°. (Schlossberg, 1900.)
Freezing-point data for mixtures of water and ammonium tartrate and of
water and ammonium racemate are given by Bruni and Finzi (1905).
AMMONIUM THIOCYANATE 70
AMMONIUM THIOCYANATE NH4SCN
SOLUBILITY IN WATER.
(Average curve from results of Riidorff, 1868 and 1872; Wassilijew, 1910; Smits and Kettner, 1912.)
to Gms. NH4SCN -,., p, « Cms. NH4SCN Solid
* ' per 100 Gms. Sat. Sol. Phase' * ' per too Gms. Sat. Sol. Phase.
-io 20 Ice o 54.5 NH4SCN
-15 28.5 +10 59
-20 35.5 20 63
-25.2 42Eutec. Ice+NH4SCN 25 65.5
-io 50 NKtSCN 30 67.5
Data for the system ammonium thiocyanate, thiourea and water at 25° are
given by Smits and Kettner (1912) in the form of a triangular diagram, but the
numerical results are omitted. The diagram confirms the freezing-point lowering
results in showing that the molecular compound NhUSCN^NH^CS is formed.
IOO gms. acetonitrile dissolve 7.52 gms. NH4SCN at l8°. (Naumann and Schier, 1914.)
Freezing-point curves have been determined for the following mixtures:
Ammonium Thiocyanate + Ammonia. (Bradley and Alexander, 1912.)
+ Potassium Thiocyanate. (Wrzesnewsky, 1912.)
+ Thiocarbamide (Thiourea). (Renolds and Werner, 1903;
Findlay, 1904; Atkins and Werner, 1912; Smits and Kettner, 1912; Wrzesnewsky, 1912.)
AMMONIUM URATE (Primary) CgHsN^NH*.
SOLUBILITY OF THE LACTAM AND LACTIM FORMS IN WATER.
(Gudzeit, 1908-09.)
Gms. of Each per 1000 cc. Sat. Solution.
Lactam. Lactim. Mixture of the Two.
1 8 0-456 0.304 0.414
37 0.817 0.540 0.741
AMMONIUM Meta VANADATE NH4VO3.
SOLUBILITY IN WATER AND IN AQUEOUS AMMONIUM SALT AND AMMONIUM
HYDROXIDE SOLUTIONS.
(Meyer, 1909.)
Gms. per 1000 cc. in Each Solvent.
18
25
35
45
55
70
loo cc. anhydrous hydrazine dissolve 2 gms. ammonium metavanadate at
room temp. (Welsh and Broderson, 1915.)
AMYGDALIN C20H27NO.3H2O.
IOO gms. trichlorethylene dissolve 0.029 gm- amygdalin at 15°.
(Wester and Bruins, 1914.)
AMYL ACETATE BUTYRATE, FORMATE, etc.
SOLUBILITY IN WATER AND IN AQUEOUS ALCOHOL AT 20°.
[(Bancroft— Phys. Rev. 3, 131, 106, 205, 'Q5-'o6; Traube. — Ber. 17, 2304, '84.)
p. t._ cc. Ester per Sp. Gr. v . cc. Ester per Sp. Gr.
loocc. H20. of Ester. 100 cc. H2O. of Ester.
Amy 1 acetate 0.2 0.88 Amyl propionate o.i 0.88
Iso amyl acetate 0.2(1.2?) ... Iso amyl formate 0.3 (gms. at 22°)
Amyl butyrate 0-06 0.85
Water.
0.05 n.
NH4C1.
o.i n.
NH4C1.
0.05 n.
NH4NO3.
o.i n.
NH4N03.
0.0668 n.
NH3.
0.245 n.
NH3.
0.588 n.
NH3.
4-35
1.66
0.41
.1.67
0.58
5-58
7-97
1 2. 06
6.08
2.63
I.I7
2.77
1.23
7.06
8.58
12.66
IO. 77
r 21
2 .60
I cj 71
8 88
5 40
IQ O7
ii 18
7 40
3O.A7
AMYL ACETATE
SOLUBILITY IN AQUEOUS ALCOHOL AT ROOM TEMPERATURE.
(Pfeiffer, 1892.)
Solubility of I so Amyl Acetate Solubility of Amyl Acetate and Amyl
in Aq. Alcohol Mixtures. Formate in Aq. Alcohol Mixtures.
Per 5 cc. C2H5OH.
cc. H2O.
cc.IsoAmyl
acetate.
7
6
0.41
0-7
3-6i
I-3I
3-o
3.01
2.60
4-0
S-o
cc.
in Mixture.
cc. H2O added to cause separation
of second phase in mixtures of the
given amounts of alcohol and 3 cc
portions of :
Amyl
Formate.
Amyl
Acetate.
3 i. 80 1.76
9 8.77 9.03
15 17.01 17.52
21 27.06 26.99
27 38-3I 37-23
33 So-71 48-41
39 65.21
45 85.10
48 94 . 20
AMYL ALCOHOL C6HUOH.
SOLUBILITY OF AMYL ALCOHOL IN WATER AT 22°.
(Herz — Ber. 31, 2671, '98.)
ioo cc. water dissolve 3.284 cc. amyl alcohol. Sp. Gr. of solu-
tion = 0.9949, Volume = 102.99 cc.
ioo cc. amyl alcohol dissolve 2.214 cc. water. Sp. Gr. of solu-
tion = 0.8248, Volume = 101.28 cc.
Sp. Gr. of H2O at 22° = 0.9980; Sp. Gr. of amyl alcohol at 22°= 0.8133.
SOLUBILITY IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL.
(Pfeiffer, 1892; Bancroft, 1895-96.)
Mixture of
Mixture of
c.c. H2O added to *
n«r* A
C6HUOH+C2HSOH
Mixture at
C.C. C.C.
9.1°.
19.2°.
3 3
3-21
3-5
3 6
IO-35
10.80
3 9
18.34
19.10
3 12
27.47
29.15
3 15
41.25
43-15
c.c. H2O Added to *
Mixture at
c.c.
3
6
9
12
15
c.c.
3
3
3
3
3
13.3 •
3.36
2. 2O
2.10
2.10
2.10
17.4°-
3-47
2.25
2.15
2.10
2.IO
.* Just enough water was added to produce cloudiness.
NOTE. — The effect of various amounts of a large number of salts
upon the temperature (39.8°) at which a mixture of 20 cc. of amyl
alcohol + 20 cc. of ethyl alcohol -f 32.9 cc. of water becomes homo-
geneous has been investigated by Pfeiffer (Z. phys. Ch. 9, 444, '92).
The results are no doubt of interest from a solubility standpoint, but
their recalculation to terms suitable for presentation in the present
compilation has not been attempted.
DISTRIBUTION OF ISOAMYL ALCOHOL BETWEEN WATER AND COTTON SEED
OIL AT 25°.
(Wroth and Reid, 1916.)
Cms. CjHuQH per ioo c.c.
Oil Layer. H2O Layer.
1.947 0.9153 0.470
2.195 I.II56 0.508
2.273 I.I050 0.486
2.372 0.9995 0-421
AMYL ALCOHOL 72
SOLUBILITY OF AMYL ALCOHOL IN WATER AND IN AQUEOUS SOLUTIONS OF
ETHYL AND METHYL ALCOHOLS.
(Fontein, 1910.)
t°.
15
20
40
60
80
IOO
120
140
1 00
170
180
187,
In Water.
Gms. CjHnOH per
ioo Gms.
H20
Layer.
C6HUOH
Layer.
4
2.6
90.7
2.6
90.6
2.1
89.5
2
88
2-5
86
3
83.8
3-8
80.8
5
76.4
7-3
70
9-3
65.1
13-5
57-3
In Aq. Ethyl Alcohol."
In Aq. Methyl Alcohol.f
Gms. CcHuOH per
Gms. CsHnOH per
to
ioo Gms.
t°.
ioo Gms.
2H5OH+]
320 CjHuQH
CH3OH+H2O CsHuOH*
Layer.
Layer.
Layer.
Layer.
4-5
16.2
. . .
3-6
II
. . .
20
20.8
. . .
20
19-3
. . .
40
26.7
. . .
38.4
. . .
78.4
60
33
. . .
40
31.2
78
67.8
24.4
50
37-i
74.8
70
36,'s
73-7
60
43-3
71.6
80
40.8
70.1
70
52.7
65
90
47
64
72
(crit.
temp.)
94.2
(crit.
temp.)
(crit. temp.)
Of 33-55 per cent QHjOH.
f Of 33 Per cent CH3OH.
The "synthetic method" was used for the preceding determinations. Fer-
mentation amyl alcohol of b. pt. I3i°-I3i.4° and ^15.5 = 0.814 was employed.
It contained 16% of optically active amyl alcohol. Many other series of deter-
minations were made with solvents containing other percentages of ethyl and
methyl alcohol. Also, other series were made for the above-named ternary
systems at constant temperatures from which binodal curves were obtained.
The author uses a very ingenious indirect method for determining the composi-
tion of the conjugated solutions. Data are also given for the distribution of
ethyl alcohol between water and amyl alcohol.
"The results of Alexejew (1886) for the solubility of amyl alcohol in water
agree fairly well with the above data.
AMYL AMINE C6HU.NH2.
The freezing-point curve for mixtures of amyl amine and water is given by
Pickering (1893).
Iso AMYLAMINE HYDROCHLORIDE C6Hn.NH2.HCl (iso).
IOO gms. H2O dissolve 192.2 gms. of the salt at 25°. (Peddle and Turner, 1913.)
ioo gms. CHC13 dissolve 5.1 gms. of the salt at 25°.
Data for the distribution of e-chloramyl amine between water and tetra-
chlorethane at o°, water and nitrobenzene at 25° and water and benzene at 25°
are given by Freundlich and Richards (1912).
AMYLENE (Trimethylethylene) (CH3)2C: CHCH3.
RECIPROCAL 'SOLUBILITY IN ANILINE; DETERMINATIONS BY SYNTHETIC METHOD.
(Konowalow, 1903.)
Gms. Aniline per ioo Gms.
Amylene Layer. Aniline Layer.
28
Gms. Aniline per ioo Gms.
Amylene Layer. Aniline Layer.
19-5
19.7
20.5
21-7
24.2
81.5
80.5
79-5
78
75-8
10
12
13
14
34
38.5
45
14.5 (crit. temp.) 51.6
73
68
64.7
59
•73 AMYLENE
SOLUBILITY OF AMYLENE IN LIQUID CARBON DIOXIDE.
(Buchner, 1905-06.)
(Determinations made by the synthetic method.)
t°. (crit.) 31 103 201
Cms. CsHio per 100 gms. sat. sol. o 38 100
AMYLENE HYDRATE (CH3)2C(OH)CH2.CH8.
• The distribution coefficient of amylene hydrate between olive oil and water
at ord. temp, is I. (Baum, 1899.)
ANDROMEDOTOXINE C3iH6iOi0.
SOLUBILITY IN SEVERAL SOLVENTS AT 12° AND AT THE BOILING-POINTS OF
THE SOLVENTS.
(Zaayer, 1886.)
Gms. CsiHjiOxo per 100 Gms. Sat. Sol. at :
Solvent. t -- - > - -,
12°. B. Pt.
Water 2.81 0.87
Ethyl alcohol (&& = 0.821) n .70
Amyl alcohol i . 14
Chloroform o . 26 o . 26
Commercial ether o . 07 o . 07
Benzine o . 004
ANETHOLE (p Propylanisole) C
SOLUBILITY IN AQUEOUS ALCOHOL AT 20°
(Schimmel and Co., Reports, Oct. 1895, p. 6.)
Vol. per cent alcohol = -20 25 30 40 50
Gm. anethole per liter aq. alcohol = 0.12 0.20 0.32 0.86 2.30
333-3 gms- anethole dissolve in one liter of 90% alcohol at room temperature.
(Squire and Caines, 1905.)
Freezing-point data for mixtures of anethole and menthol are given by Scheuer
(1910).
ANILINE C6H6(NH2).
SOLUBILITY IN WATER AT 22°.
(Herz, 1898; see also Vaubel, 1895; Aignan and Dugas, 1899.)
loo cc. H2O dissolve 3.481 cc. C6H5(NH2) — Vol. of Sol. = 103.48, Sp. Gr. =
0.9986.
100 cc. C6H6(NH2) dissolve 5.22 cc. H2O — Vol. of Sol. = 104.96, Sp. Gr. =
1.0175.
100 cc. sat. aq. sol. contain 3.607 gms. C6H5NH2 at 25°. (Reidel, 1906.)
SOLUBILITY OF ANILINE IN WATER. (Determination by synthetic method.)
(Sidgwick, Pickford and Wilsden, 1911.)
to Gms. QHSNH2 per 100 Gms. Gms. QHiNHz per^ioo Gms.
Aq. Layer. Aniline Layer. Aq. Layer. Aniline Layer.
13.8 3-6lI 5.12 (200) 120 Q.I 14.6
3° 3-7 5-4 130 ii-2 16.9
50 4.2 6.4 140 13.5 19.5
70 5 7.7 150 17.1 24
9O 6.4 9.9 l6o 22 32
no 8 13 165 26.1
The critical solution temperature for aniline and water is 168°.
Alexejew (1886) and Rothmund (1898) obtained results for the preceding
system which differ in part quite widely from the above table.
More recent determinations, in terms of cc. aniline per IOO cc. of mixture, are
given by Kolthoff (1917).
ANILINE
74
SOLUBILITY OF ANILINE IN AQUEOUS SOLUTIONS OF ANILINE HYDROCHLORIDE.
(Sidgwick, Pickford and Wilsden, 1911.)
The temperatures at which a second liquid phase separated from homogeneous
mixtures of known amounts of aniline + HC1 + H2O were determined for a very
extensive series of mixtures. The procedure consisted in first heating a given
mixture until it became homogeneous and then cooling it slowly, with constant
shaking. A critical turbidity preceding the actual separation by a few de-
grees was always noticed. The point of separation was taken as that at which
a small gas flame seen through the liquid disappeared. At higher temper-
atures, the observations were made on mixtures contained in sealed bulbs. In
the actual experiments, binodal curves for mixtures of Aq. HC1 (of different
strengths) and aniline were determined. By interpolation from these, the fol-
lowing isothermal curves were obtained.
Isotherm for 15°.
Isotherm for 25°.
H2O Rich Mixtures.
Gms. per 100 Cms.
Sat. Solution.
Aniline Rich Mixtures. '
Gms. per 100 Gms.
Sat. Solution.
H2O Rich Mixtures.
Gms. per 100 Gms.
Sat. Solution.
Aniline Rich Mixtures.
Gms. per 100 Gms.
Sat. Solution.
C6H5NH2. C6H5NH2.HC1.
H2O. C6HBNH2.HCi.
C«H6NH2. C,H6NH2.HC1. ' H2O. C6H5NH2.HC1.
3-6IS
0
7
.276
3
.025
3
.681
0
14
8.884
3-7QI
1-529
7
.231
i
.989
4
.020
3.02
10.
84
6.062
4.144
5.829
5
.816
i
• 195
5
.380
ii .40
6.
949
1.912
4.940
11.44
5
.230
o
•340
7
.023
15-83
6.
043
0.828
5-995
16.03
5
.006
0
.163
ii
.86
19.02
5-
568
0-363
10.44
19-35
4
.960
0
.080
3i
•35
20.15
5-
3H
0.089
26.80
21.49
4
.942
o
59
•95
15-55
5-
299
0
9-30
21.21
Isotherm for 40°.
Isotherm for 60°.
3-941
0
15-65 8
•752
4.58
0
14
.27
5-93
4-i87-
i
523
10
.21
4
.243
4.87
1.512
9
.569
2.632
4-371
3
009
7
.874
2
.166
5.13
2.984
8
.109
1. 112
4.823
e
815
7
.069
I
.452
5.67
5.762
7
•492
0.4876
6.2IO
II .
30
7
.058
0
.9669
7.69
II .14
7
.051
0.2284
8.779
15
55
6
.225
0
-4052
n-53
15-25
7
.047
O.II38
38.69
18
5
.940
0
.0960
22.80
16.66
7
.030
0
64.20
12
.84
5
•930
0
51.10
14.36
Isotherm for 8e°.
Isotherm for 100°.
5-66
o
12
•31
3-387
7
.10
0
41-57
n-45
5-95
i
•495
9
.848
1-35°
7
.68
I
.467
18.16
4-995
6.26
2
•950
8
.998
0-5857
8
.10
2
.891
12.76
1.784
7.11
5
.678
8
-524
0.2769
9
.60
5
.522
n-37
0.1836
9-95
10
•85
8
.512
0.1387
13
.60
10
.41
11.90
0
31.18
14
•85
8
.500
0
Isotherm for 120°.
o 17-94
9.497 14.45
2-459
o
T3-75
38.75
Isotherm for 140°.
o 29-52 4.043
7-384 21.09 o
The authors also calculated the position of tie lines for the binodal curves
with the aid of distribution coefficients, which they determined at 25 and which
are quoted in a subsequent table (page 78 following).
Additional data for the system aniline + HC1 + H2O at o°, 25° and at 35
are given by Thonus (1913), and for aniline -f HC1 by Leopold (1910).
75 ANILINE
SOLUBILITY OF ANILINE IN AQUEOUS SALT SOLUTIONS AT 18°.
(Euler — Z. physik. Chem. 40, 307, '04.)
Aq. Solution. Cms. Salt Cms, C6H5(NH2) Aq. Cms. Salt Cms. C«H6(NH2)
per liter, per 100 g. solvent. Solution. per liter, per looitsolvent!
H2O alone o 3.61 i wNaOH 40.06 1.90
o.5wKCl 37.3 3.15 i wLiCl 42.48 2.80
iwKCl 74.6 2.68 iwCaCl2 67.25 3.00
iwNaCl 58.5 2.55
SOLUBILITY OF ANILINE IN AQUEOUS ANILINE HYDROCHLORIDE
SOLUTIONS AT 18°.
(Lidow — J. russ. phys. chem. Ges. 15, 420, '83; Ber. 16, 2297, '83.)
Per cent C6H6NH2HC1 Cms. CeNsNHz Per cent C6H5NH2JIC1 Cms. CeHsNHj
insolvent, per 100 g. Solvent in Solvent. per loog? Solvent.
5 3-8 30 39.2
5-3 35 So-4
SOLUBILITY OF ANILINE IN AQUEOUS SOLUTIONS OF GLYCEROL AND
VICE VERSA.
(Kolthoff, 1917.)
(The liquids were measured from burets. The determinations at 100° were
made in sealed tubes. The others were made in open tubes.)
Results for the Solubility of Aniline in Aqueous Glycerol.
Per cent Glycerol in
Aq. Mixture used.
cc. Am
line dissc
lived by
ioo cc. of Aq. G
Uycerol of Com
:. shown at:
18°. 25°.
36°.
r 00°.
o (= water)
3
•25
3
•4
5-6
9.9
39
5
•15
5
•3
. . .
56
7
•5
7
.6
28 (58*
7o Glycerol)
65
10
.
38 (66<
7o " )
74-3
ii
•75
12
.1
. . •
. . .
78
20
2O
16
...
87
70
.
. . .
Results for the Solubility of Aqueous Glycerol in Aniline.
Per cent Glycerol in CC- °* Aq> Glycerol Mixture dissolved by too cc. Aniline at:
Aq. Mixture used.
o (= water)
39
47
56
74-3
DISTRIBUTION OF ANILINE BETWEEN WATER AND BENZENE AT 25°.
(Farmer and Warth, 1904.)
Cms. C6H5NH2 per 100 cc.
Ratio.
18°.
25°-
36°.
IOO .
4.6
5
4
5-3
6.4
5-2
. . .
• • •
...
7-9
7-7
. . .
15 (58% Glycerol)
I3-I
11.7
...
17(66% " )
I7.I
14.8
Water Layer. C6H6 Layer.
0.0135 O.I3I2 9.7
0.0122 0.1282 10.5
0.0065 0.0656 10. i
.Data for the distribution between water and benzene at 25° of each of the fol-
lowing substituted anilines; o, m and p nitraniline, chloraniline, bromaniline,
P nitrosmethylaniline, and p nitrosodimethylaniline are given by Farmer and
Warth (1904).
ANILINE 76
SOLUBILITY OF ANILINE, PHENOL MIXTURES IN WATER.
(Schreinemaker — Z. physik. Chem. 29, 584; 30, 460, '09.)
Mitture used = 2^.4 Mols. Aniline
+ 74 6 Mols. Phenol „
Mixture used = 50 Mols. Aniline
+ 50 Mols. Phenol
• « Gms. of Mixture per ioo Gms. * •
Gms. of Mixture per ioo Gms.
*^Aq. Layer. A.
+ P . Layer.
Aq. Layer. A,
, + P. Layer.
40
5-o
86-0
40
4-0
91-5
60
55
82.0
80
5-5
85 5
80
8.0
77 o
IOO
8.0
82 o
IOO
12 5
67 o
120
13 5
73 5
no
19.0
56.5
130
19.0
66 o
104
(crit. temp.) 33
23 5
58.0
140
(crit. temp.) 35
Determinations in above table by "Synthetic Method," see NOTE, p. 16.
Schreinemakers gives results for several other mixtures of aniline and phenol
which yield curves entirely similar to those for the two mixtures here shown.
DISTRIBUTION OF ANILINE BETWEEN:
(Vaubel — J. pr. Chem [2] 67, 477, '03.)
Water and Ether. Water and Carbon Tetrachloride.
Composition of Solutions. Gms. CeHsNHain: Com position jof Solutions. Gms.C6H6NH2 in:
G.CeHfiNHa ^ Aq. EtLer G. CeHgNHa " gl ' Aq. ' CCU '
Used. Layer. Layer. Used. Layer. Layer.
1.2478 50 cc. H2O 50 cc. H2O
+ 2occ. Ether 0.1671 1.0807 °«3478 +2occ.CCl4 0.33580.012
1.2478 50 cc. H2O 50 cc. H2O
+ 50 cc. Ether 0.0835 1.1643 1.2478 +5occ. CC14 0.2767 1.971
1.2478 50 cc. H2O 50 cc. H2O
4- 1 oo cc. Ether 0.0594 1.1884 1.2478 +ioocc. CC14 0.1845 1.063
SOLUBILITY OF ANILINE IN SULPHUR.
(Alexejew — Ann. Physik. Chem. 28, 305, '86.)
. loog. Gms. C6HsNH2 per loog.
S. Layer. Anilin Layer. S. Layer. Anilin Layer.
ioo 4 75 *3Q I5 58
no 6 70 135 17.5 47
120 10 64 138 (crit. temp.) 23 . .
DISTRIBUTION OF ANILINE BETWEEN WATER AND TOLUENE AT 25°.
(Riedel, 1906.)
NOTE. — Mixtures of aniline and toluene were shaken with water and after
separation of the two layers the Sp. Gr. of the A : T mixture (layer) was de-
termined and also the amount of aniline in each layer.
Solution Shaken with
A : T Mixture.
Vol. per cent Sp. Gr. of A : T
Aniline : Toluene Mixture after
in Mixtures Used . Separation .
Gms. C6H5N
H2 in ioo cc. c
A : T Layer.
Aq. Layer.
HaO
50:50 0.9257
41-5
2.14
u
25:75 0.8928
20-7
I .5
tt
12.5:87.5 0.8737
8.62
0.86
ti
5.5:94.5 0.8661
3-87
o 45
"
2.5:97.5 0.8627
1.68
0.21
The author also gives data for the distribution of aniline between toluene
and aqueous solutions of K2SO4, KBO3, Ba(OH)2, Sr(OH)2 and Ca(OH)2.
77
ANILINE
SOLUBILITY DATA DETERMINED BY THE FREEZING-POINT METHOD (see foot-
note, page i) ARE GIVEN FOR MIXTURES OF ANILINE (m. pt. —5.5° to —6.8°)
AND OTHER COMPOUNDS.
Name and M. Pt. of the Other Com-
pound of Each Mixture..
Nitrosodimethyl aniline (85.5°)
Benzene (5.42°)
Nitrosobenzene (63.5°)
Nitrobenzene (2.8°)
o Dinitrobenzene (116.5°)
m (91°)
P
s Trinitrobenzene (122.2°)
o Chloronitrobenzene (32°)
» (43°)
P " (82.5°'
Benzoic acid (121.25°)
Chloroform (-63°)
o Cresol (30.4°)
m " (4.2°)
P " (33-2°)
Ethylacetate (-83.8°)
Hydroquinone
Allyl mustard oil
o Chlorophenol
o Nitrophenol (46°)
m (96°)
P " (H3°)
m Dinitrophenol (110.5°)
Pyrocatechol (105°)
Resorcinol (110°)
Nitrotoluene (51.3°)
Dmitrotoluene (71°), 1.3.4; 1.3.
and 1.2.6
Trinitrotoluene (82°)
Isopentane (less than — 24°)
Data for First Eutectic.
M. Pt.
- 9.2
-12.5
— 30.6
— 10
- 8
Wt. Per Cent.
QH5NH2.
94- 2 '
77.2
53-4
92.2
92.7
no eutectic
not determined 3
— 19.5 66.1
-12.6 79.7
-16.3 72.7
-71
-17
-30
-IS-
'89
21.7
78. 84
74- 3s
85- S6
62"
7
-13.5 80.2
-18.7 74. 28
-17.5 86. 8»
- 7-3 94- S10
-13 86. 5 u
not determined
-17 89
5 | -13., 80.8
- 8 96. 412
Authority.
(Kremann, 1904.)
(Kremann and Borjanovics, 1916.)
(Kremann, 1904.)
(Kremann and Rodinis, 1906.)
(Kremann. 1904.)
(Kremann and Rodinis, 1906.)
(Kremann, 1904.)
(Kremann, 1907.)
(Kremann and Rodinis, 1906.)
(Baskov, 1913.)
(Tsakalatos and Guye, 1910.)
(Kremann, 1906.)
(Kremann, 1906; Philip, 1903.)
(Wroczynski and Guye, 1910.)
(Kremann and Rodinis, 1906.)
(Kurnakov and Kriat, 1913.)
(Kurnakov and Solover, 1916.)
(Bramley, 1916.)
(Kremann and Rodinis, 1906.)
(Kremann. 1906.)
((Kremann and Rodinis. 1906.)
(Kremann, 1904.)
(Kremann. 1906.)
(Campetti and del Grosso, 1913.)
1 A second eutectic melts at 76° and contains 7 per cent C6H6NH2, a molecular compound of m. pt. 92°
and containing 24 per cent C6H5NH2 exists between these eutectics. The author also gives data for the
effect of nitrobenzene, o nitrophenol and of m xylene upon the lowering of the m. pt. of the above com-
pound. 2 A break in the curve at 41.5° and 39.2 per cent QHsNHj indicates that a molecular compound
exists between the first eutectic and this point. • The first eutectic apparently lies too near pure aniline
to be determined. An equi-molecular compound of aniline and s trinitrobenzene (m. pt. 30°) exists over
the range pure aniline to the" second eutectic which melts at 101° and contains 8.7 per cent QHsNHj.
4 A second eutectic melts at o and contains 28.7 per cent C6H5NH2, the molecular compound between
these points melts at 8.3° and contains 46.2 per cent C8HSNH2. 5 A second eutectic melts at —31° and
contains 17 per cent C6H8NH2, the molecular compound between these points melts at —14.6° and con-
tains 49 per cent C6H6NH2. • The second eutectic melts at 6° and contains 23 per cent QH6NH2, the
molecular compound melts at 19.2° and contains 47.5 per cent C6H5NH2. 7 There are two eutectics
between which an equi-molecular combination exists. 8 There is a break in the curve at 26° and 421.
per cent C6HBNH2 indicating the existence of a molecular compound from the eutectic up to this point.
9 There is a break in the curve at 42° and 39.8 per cent CtHsNH* indicating formation of a molecular
compound. » There is a break in the curve at 74° and 32.9 per cent C6H5NH2 indicating the existence of
a molecular compound from the eutectic up to this point. " There is a break in the curve at 39° and
48.9 per cent CeHBNH2. « A second eutectic melts at 60° and contains 7 per cent CsHjNHz, the molec-
ular compounds melts at 85° and contains 30 per cent QHsNHg.
ANILINE 78
RECIPROCAL SOLUBILITY OF ANILINE AND HEXANE.
(Keyes and Hildebrand, 1917.)
t° of Complete Gms. Hexane per 100 t° of Complete Gms. Hexane per 100
Miscibility. Gms. Mixture. Miscibility. Gms. Mixture.
26.1 9-6 59-2 35-9
43.9 14.8 59.4 41-6
45.9 16.3 59.6 48
49-9 20 57.9 62.9
Si-4 21 53.9 73.1
56 27.2 47.2 80.6
58.2 31 35-6 88.1
58.2 34-6 16.5 93.8
RECIPROCAL SOLUBILITY OF ANILINE AND PHENOL, DETERMINED BY THE
FREEZING-POINT METHOD.
(Schreinemakers, 1899.)
Mols. C6H5NH2 Mols. C6H5NH2
t° of Melting. per 100 Mols. Solid Phase. t° of Melting. per 100 Mols. Solid Phase.
Mixture. Mixture.
— 6.1 loo C6H5NH2 3o.4m.pt. 50 1.1
- 8.9 96 " 28.6 40
— n.7Eutec. 92.3 c6H6NH2+i.i 22.3 30
— 6.5 90 i.i 14.8 EuteC. 21.2 i.i+C«H6OH
+ 10. 1 80 " 18.4 20 QH5OH
22 70 " 31.4 10
28.5 60 " 37.3 4
i.i = C6H5NH2.C6H6OH.
Data for* the solubility of aniline in cyclohexane at pressures up to 300 at-
mospheres are given by Kohnstamm and Timmermans (1913).
ANILINE HYDROCHLORIDE C6H6NH2.HC1.
IOOCC. H2O dissolve 17.8 gms. of the salt at 15°. (NiementowskiandRoszkowski, 1897.)
IOO gms. H2O dissolve IO7.I gms. of the salt at 25°. (Peddle and Turner, 1913.)
ioo gms. sat. solution in water contain 52.1 gms. C6H6NH2.HC1 at 25°.
loo gms. sat. solution in aniline contain 8.89 gms. CeHsNHg.HCl at 25°.
(Sidgwick, Pickford and Wilsden, 1911.)
DISTRIBUTION OF ANILINE HYDROCHLORIDE BETWEEN WATER AND ANILINE AT 25°.
(Sidgwick, Pickford and Wilsden, 1911.)
O.II
O.2
0-3
0.4
0.5
C»q. = gms. salt per ioo gms. aq. layer. C»n. = gms. salt per ioo gms. ani-
line layer.
NitrANILINES C6H4NH2NO2. o, m, and p.
SOLUBILITY IN WATER.
(Carnelly and Thomson — J. Chem. Soc. S3. 768, '88; Vaubel — J. pr. Chem. [2] 52, 73. '95', above ao°,
Lowenherz — Z. physik. Chem. 25, 407, '98.)
" Grams Nitraniline per Liter of Solution.
Ortho Nitraniline. Meta Nitraniline. Para Nitraniline.
20 ... 1.14-1.67 0.77-0.80
24-2 1.25 (25°) 1.205
27.3 ... 1.422
IOO CC. H2O dissolve 2.2 gms. p nitraniline at IOO°. (Jaeger and Kregten, 1912.)
C»n.
c^
'CM.
c.q.
C»n.
c*
./c...
C»q.
<
-M.
Caq./Can.
0.006
19
•30
0.6
0
.219
2
•74
I
o
.804
1.24
O.O2O
10
0.7
0
•327
2
.14
I.I
I
.005
I
0.043
6
.98
0.8
o
.471
I
.70
1.2
I
.228
0.98
0.086"
4
•65
0.9
o
.631
I
•43
i-3
I
.412
0.92
0.146
3
.42
79 NitrANILINES
SOLUBILITY OF ORTHO AND OF META NITRANILINE IN HYDROCHLORIC
ACID.
(Lowenherz.)
Ortho Nitraniline at 25°. Meta Nitraniline.
G. Mols. per Liter.
Grams
_ger_
Liter.
G. Mols. per Liter.
Grams
per Liter.
'HCl
o.o
0.63
1.26
C6H6NH2.
N02(o)
O.OO9I
0.0143
0.0174
0.021^
HCl
o.o
22.97
34-63
45-94
N02(<7)2'
1-25
1.97
2.40
2.97
(25°)
(26-5°)
(23-3°)
O
O
O
HCl
• O
.OI25
.0247
NO2(w)
0-0091
0.0183
0.0274
HCl
o.o
0.46
0.90
1. 2O
2-S3
3-85
SOLUBILITY DATA DETERMINED BY THE FREEZING-POINT METHOD ARE GIVEN
FOR THE FOLLOWING MIXTURES.
o Nitraniline + m Nitraniline \
«« , «< f (Kremann, 1910; Valeton, 1910; Holleman, Hartogs
• * I and van der Linden, 1911, Nichols, 1918.)
m + p '
o " 4- o Nitracentanilide (Jaeger, 1906.)
p + p Nitrosoaniline (Jaeger and van Kregten, 1912.)
0 + Benzene (Bogojawlensky, Winogradow and Bogalubow, 1906.)
m' " +
p ."_[_" « « U
o " + Nitrobenzene " " «•
m » +
p " _1_ " « « €i
o " + Ethylenebromide
m " +
p '« _i_ » " « ««
m + m Dinitrobenzene (Crompton and Whitely, 1895.)
m -\- s Trinitrobenzene (Smith and Walts, 1910; Sudborough and Beard, 1910.)
p « + 5
m + Naphthalene (Pushin and Grebenschikov, 1913.)
O " + Phenol (Kremann and Rodinis, 1906.)
m " + "
P » + »
s Tribromaniline + 2 Chlor, 4.6 Dibromaniline (Sudborough and Lakhamalani, 1917.)
p Nitroethylaniline + p Nitrosoethylaniline (Jaeger and van Kregten, 1912.)
p " propylaniline + p Nitrosopropylaniline
Nitrodiethylaniline + Nitrosodiethlyaniline (Jaeger, 1905, 1907.)
Methylaniline + Benzylchloride (Wroczynski and Guye, 1910.)
Dimethylaniline + Benzene (Schmidlin and Lang, 1912.)
+ Tetramethyldiaminobenzophenone
" + Phenol (Bramley, 1916; Kremann, 1906.)
+ o Chlorophenol (Bramley, 1916.)
Tetranitromethylaniline + a Trinitrotoluene (Giua. 1915.)
+ P Nitrotoluene
Nitrosodimethylaniline + 0 Naphthylamine (Kremann, 1904.)
4- Phenol
+ o Toluidine
+ p «
" + m Xylidine
NitrANILINE 80
SOLUBILITY OF META AND or PARA NITRANILINE IN ORGANIC
SOLVENTS AT 20°.
(Carnelly and Thomson.)
Gms. per Liter. Solvent Cms, per Liter.
Meta. Para. Meta. Para.
Methyl Alcohol no. 6 95.9 Benzene 24.5 19.8
Ethyl Alcohol 70 . 5 58.4 Toluene 17.1 13.1
Propyl Alcohol 56.5 43.5 Cumene "-5 9-o
Iso Butyl Alcohol 26 . 4 19.1 Chloroform 30 . i 23 . i
Iso Amyl Alcohol 85 . i 62 .9 Carbon Tetra Chloride 2.1 1.7
Ethyl Ether 78.9 61.0 Carbon Disulfide 3.3 2.6
ANILINE SULFATE C6H6NH2.H2SO4,
loo cc. H2O dissolve 6.6 gms. C6H5NH2.H2SO4 at 15°.
(Niementowski and Roszkowski, 1897.)
ANISIC ACID (£-Methoxybenzoic Acid) CH3O.C6H4COOH.
1000 cc. sat. aqueous solution contain 0.2263 gm. acid at 25°. (Paul, 1894.)
SOLUBILITY OF ANISIC ACID IN SEVERAL ALCOHOLS.
(Timofeiew, 1894.)
In Methyl Alcohol. In Ethyl Alcohol. In Propyl Alcohol.
Gms. per 100 Gms. Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol. " Solvent. Sat. Sol. " Solvent. Sat. Sol. Solvent!
o 51.1 104.5 46.7 87.6 35 53.8
16.5 64.9 183.5 53.6 115.5 43 75.5
Data for the distribution of anisic acid between water and olive oil at 25°
are given by Boeseken and Waterman (1911, 1912).
pANISIDINE C6H4(OCH3).NH2.
DISTRIBUTION BETWEEN BENZENE AND WATER AT 25°.
(Farmer and Warth, 1904.)
Gms. C6H4(OCH3).NH3 per 100 cc.
QHfi Layer. H2O Layer.
0.4356 0.0747
0.6662 O.III2
O.9OIO O.I472
ANISOLE C6H6OCH3.
RECIPROCAL SOLUBILITY OF ANISOLE AND BENZYL CHLORIDE DETERMINED
BY THE FREEZING-POINT METHOD.
(Wroczynski and Guye, 1910.)
« nf Gms. C6H5OCH3 ~ llV1 « nf Gms. C
—37.2 ioo QHsOCH, — 72.8Eutec. 46.1
— 40 93.3 " —60 28 C6H5CH2C1
-50 75-3 -50 13
— 60 62.1 " —41.1 o
p NitrANISOLE
FREEZING-POINT CURVES (Solubilities, see footnote, page i) ARE GIVEN FOR
THE FOLLOWING MIXTURES.
p Nitranisole + Mercuric Chloride (Mascarelli, 1908, 1909; Mascarelli and Ascoli, 1907.)
" _j_ Urethan (Mascarelli, 1908, 1909; Pushin and Grebeuschukov, 1913.)
" + " + HgCl2 (Mascarelli, 1908, 1909.)
-f Diphenylamine (Pushin and Grebenschukov, 1913.)
Dinitranisole -f- Dinitrophenetol (Blanksma, 1914-)
8i
ANTHRACENE
ANTHRACENE Ci4H10
SOLUBILITY OF ANTHRACENE IN SEVERAL SOLVENTS.
Solvent. t° «^f|j£. Authority.
Ethyl Alcohol (abs.) 16 0.076 (v. Becchi.)
" " " 19-5 I-9 (de Bruyn, 1892.)
". " " 25 0.328 (Hildebrand, Ellefson and Beebe, 1917.)
" " " b. pt. 0.83 (v. Becchi.)
Methyl Alcohol (abs.) 19.5 1.8 (de Bruyn 1892)
Benzene 25 1.86 (Hildebrand, Ellefson and Beebe, 1917.)
Carbon Bisulphide 25 2.58
Carbon Tetrachloride 25 0.732
Ether 25 1.42
Hexane 25 0.37
95% Formic Acid 18.3 0.03 (Aschan, 1313.)
Toluene 16.5 0.92 (v. Becchi.)
" loo 12.94
Trichlorethylene 15 I.OI (Wester and Bruins, 1914.)
SOLUBILITY OF ANTHRACENE IN BENZENE AND IN MIXTURES OF BENZENE
AND PENTANE AND OF BENZENE AND HEPTANE.
(Tyrer, 1910, and private communication. See Note, p. 447.)
Tn „ In Benzene -f- Pen- In Benzene + Heptane
In Benzene. tane at I5<> at ^o and ^
t°.
d. of Sat. Sol.
Gms. C^HIQ
per 100 Gms.
insol-
Gms. C14H,0
per loo Gms.
Solvent.
Gms. QHio per 100 Gms.
Solyent \
Solvent.
vent.
Solvent.
at 14°.
at 70°.
0
0.9008
0.605
O
0.184
0
0.2IO
1.67
10
o . 8909
o-975
10
0.225
12-5
0.284
2.10
,20
0.8812
i-43
20
0.279
25
0.372
2.64
30
0.8717
2.03
30
o-357
37-5
0.474
3.23
40
0.8627
2.78
40
0.447
50
0.592
3-87
50
0.8541
3-75
50
0-549
62.5
0.718
4-59
60
o . 8460
5-i4
60
0.600
75
0.850
5-37
70
0.8374
7
70
0.780
87.5
0.976
6.15
75
0-8347
8-35
80
0.915
IOO
I.lSo
6-93
90
1.059
IOO
i. 221;
Results for the solubility in benzene, differing from the above in some cases by
15%. are given by Findlay (1902).
SOLUBILITY OF ANTHRACENE IN ALCOHOLIC PICRIC ACID SOLUTIONS
AT 25°.
(Behrend — Z. physik. Chem. 15, 187, '94.)
Solid Phase
Anthracene Picrate
«
a
N
Anthracene Picrate
-f Picric Acid
Picric Acid
Grams per 100 Grams
Solution.
Grams per 100 Gms.
Solution.
^Acicf Anthracene
Add. Anthracene.
O
o
.176
Anthracene
3
•999
o
.202
I
.017
o
.190
it
5
.087
0
.180
2
.071
0
.206
14
5
•843
0
.162
2
•673
0
.215
(I
6
.727
0
•151
3
•233
o
.228
ftf
7
•511
o
.149
3
.469
0
.236
Anthracene and
7
•452
0
Anthracene Picrate
ANTHRACENE
82
SOLUBILITY IN LIQUID SULFUR DIOXIDE IN THE CRITICAL REGION.
(Centnerswer and Teletow, 1903.)
Weighed amounts of anthracene and liquid SO2 were placed in glass tubes
which were sealed and rotated at a gradually increasing temperature, and the
point observed at which the solid disappeared.
Gms CnHi.
100 Gms. !
40.1
45.8
47-9
2. II
2.48
2.65
65
78.2
88
Gms. CMHio per
loo1 Gms. SO,.
9-9
12.7
too Gms.
4 98
5-66 99.1
7.14 106.5
Freezing-point curves are given for mixtures of anthracene and each of the fol-
lowing compounds: Diphenyl, diphenylamine, a and /3 naphthylamines, a and /3
naphthols, resorcinol, p toluidine and triphenyl methane (Vignon, 1891); Naph-
thalene (Vignon and Miolati, 1892); Phenanthene (Vignon, 1891, Garelli, 1894);
Picric acid (Kremann, 1905).
ANTHRAQUINONE (C6H4)2(CO)2.
SOLUBILITY IN LIQUID SULFUR DIOXIDE IN THE CRITICAL REGION.
(Centnerswer and Teletow, 1908.) (See Anthracene, above.)
Gms. CuHgOi! per
100 Gms. SO2.
5.60
7-53
9.60
12.70
18.30
100 parts of absolute ethyl alcohol dissolve 0.05 part anthraquinone at 18°
and 2.249 parts at b. pt. (v. Becchi.)
loo gms. alcohol dissolve 0.437 gni. anthraquinone at 25°.
(Hildebrand, Ellefson and Beebe, 1917.)
SOLUBILITY OF ANTHRAQUINONE IN BENZENE AND IN CHLOROFORM.
(Tyrer, 1910.)
In Benzene. In Chloroform.
jo Gms. CMH8O2 per f e Gms. CUH8O2 per f 0
100 Gms. SO2. 100 Gms. SO2.
3.96
0.64
92.1
2.81
118.5
51-5
0.88
101.4
3-67
141.6
67.9
1.73
106.3
4.23
160
82.4
2.24
108.7
4.40
179
183-7
t°.
Sp. Gr. Solution.
Gms. Ci4H8O2 per
100 Gms. C6He.
t°. Sp. Gr. Solution.
Gms. C14H8O2 per
loo Gms. CHC13.
o
0.8900
O.IIO
0
-5244
0.340
20
0.8794
0.256
10
.5046
0-457
30
0.8692
0-350
20
.4850
0.605
40
0.8591
0.495
30
.4656
0.780
50
0.8439
0.700
40
.4461
0.994
00
0.8389
0.974
50
.4261
1.256
70
0.8288
1-355
55
.4164
1-415
80
O.8I90
1-775
00
.4070
1-577
SOLUBILITY OF ANTHRAQUINONE IN A MIXTURE OF CHLOROFORM AND
HEXANE AT 12.6° AND 49°.
(Tyrer, 1910, also private communication. See Note, p. 447.)
O
IO
20
30
SO
Gms. CuH^ per too Gms.
Solvent at:
%CHCl,in
Solvent.
60
90
100
Gms. CuHjOj per 100 Gms.
Solvent at:
12.6°.
O.OO6
0.016
0.024
0.034
0.068
49.0°.
0.056
0.074
0.096
0.124
0.212
12.6°.
O.IOI
0.148
O.222
0-334
0.482
49 .0°.
0.292
0.417
0.6o8
0.852
I.2O9
83 ANTHRAQUINONE
SOLUBILITY OF ANTHRAQUINONE IN ETHER.
(Smits — Z. Electrochem. pi 663, '03.)
Weighed amounts of ether and anthraquinone were placed in glass
tubes which were then sealed. The temperature noted at which the
anthraquinone disappeared and also at which the liquid phase disap-
peared (critical temp.). The two curves cross at 195° and again at
241°. Between these two temperatures the critical curve lies below
the solubility curve, hence for this range of temperature no solubility
curve is shown. The following figures were read from the curves, and
are therefore only approximately correct.
Cms. CuHgOa Cms. C
t*. per too g. t°. per 100 g. t . per 100 g.
Solution. Solution. Solution.
130 3 241 30 260 80
150 4 245 40 270 90
170 4-5 247 So 275 100
195 5.0 250 60
100 parts of toluene dissolve 0.19 part anthraquinone at 15° and 5.56 parts at
100° (v. Becchi).
loo gms. ether dissolve o 104 gm. anthraquinone at 25°.
(Hildebrand, Ellefson and Beebe, 19170
Data for the solubility of anthraquinone in mixtures of phenol and water
are given by Timmermanns (1907).
Hydroxy ANTHRAQUINONES C6H4 < (CO)* > C6H3OH.
1000 cc. H2O dissolve 0.0035 gm. a oxyanthraquinone at 25°. (Huttig, 1914.)
1000 cc. H2O dissolve o.oon gm. £ oxyanthraquinone at 25°.
1000 cc. H2O dissolve 0.000012-0.000062 gm. 1.4 dioxyanthraquinone (= chin-
izarin) at 25°.
1000 cc. H2O dissolve 0.00158 gm. 1.6 dioxyanthraquinone ( = chrysazin) at 25°.
(Huttig, 1914.)
ANTHRAFLAVINE (2.6 Dioxyanthraquinone) Ci2H6(CO)2(OH)2.
1000 cc. H2O dissolve 0.0003 Sm- anthraflavine at 25°. (Huttig, 1914.)
ANTHRARUFINE (1.5 Dioxyanthraquinone) Ci2H6(CO)2(OH)2.
looo cc. H2O dissolve 0.000285 gm. anthrarufine at 25°. (Huttig, 1914.)
ANTIMONY Sb.
Fusion-point data for mixtures of antimony and iodine are given by Jaeger
and Dornbosch (1912); for mixtures of antimony and sulphur by Jaeger and
Van Klooster (1912), and for mixtures of antimony, iodine and arsenic by
Quercigh (1912).
ANTIMONY TriBROMIDE SbBr,.
SOLUBILITY IN BENZENE DETERMINED BY "SYNTHETIC METHOD."
(Menschutkin, 1910.)
Gms. SbBr3 Gms. SbBr3
t°. per loo Gms. Solid Phase. t°. per 100 Gms. Solid Phase.
Sat. Sol. Sat. Sol.
5 . 6 m. pt. O QH, 90 83 2SbBr,.CA
4 . 5 Eutec. 8 . 3 c8H6+2sbBr3.c(lH(1 92.5111. pt. 90 . 2
15 12.5 aSbBrs-QH, 91.5 Q2.8 "
35 23 " 90 93.8
55 39 85 EuteC. 96.3 2SbBr,.C6H6+SbBr,
75 60.5 " QO 98 SbBr,
85 74.3 "94 ioo
ANTIMONY TriBROMIDE
84
RECIPROCAL SOLUBILITIES OF ANTIMONY TRIBROMIDE AND VARIOUS
ORGANIC COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1911.)
SbBr3 + Acetic SbBr3 4- Benzoic
SbBr3 4- Benzoyl
SbBr3
+ Benzene
Acid.
Acid.
Chloride.
Sulphonic Acid.
r.
Gms. SbBr3
per loo Gms.
Sat. Sol.
r.
Gms. SbBr8
per loo Gms.
Sat. Sol.
t'.
Gms. SbBr3
per 100 Gms.
Sat. Sol.
t°.
| Gms. SbBr3
per 100 Gm.
1 Sat. Sol.
16.5*
0
120*
o
- 0-5
* 0
52.5
* 0
is
12.2
"5
20. 1
— 3
19-5
So
15.8
10
41.8
no
36.8
— 6 f
32
47-5
26.2
4t
S8.2
105
50
+10
41.2
44 t
36.9
20
64.3
IOO
61.5
20
47-5
So
39-1
40
72-5
95
71
30
54
60
45-7
60
81.9
85
83.1
40
60.8
70
55-2
70
97.1
79 t
87.6
5°
67.8
80
68.1
80
92.4
85
92
60
74-9
85
77.6
90
97-8
90
96.4
80
89.4
90
90-3
94
IOO
94
IOO
94
IOO
94
IOO
Molecular compounds are not formed in the above systems. The diagram in
each case consists of two arms meeting at the eutectic.
SbBr3
+ Acetophenone.
Gms. SbBr3 ^VA
SbBr3 + Amylbenzene.
Gms. SbBr3 ^^A
SbBr3 + Anisole.
Gms. SbBrs c^i:j
t°. i
»er 100 Gr
ns' Phase.
t°. pei
"- r?°s I™3' Phase.
t°. pei
: loo Gr
081 Phase.
19-5*
O
C6H6COCH3
— 70
4.5 SbBrjj.CgHfj.CjjHu
-34*
o
C6H5OCH3
15
22.7
"
-50
8-3
-35
2.5
"-fi.i
i.S*
48.6
" +1.1
-30
16.6
— 20
11.7
i.i
20
56.8
i.i
-25
21 "
0
26.5
"
30
63.3
"
-17 t
32.5 "+SbBr3
10
37-i
"
37-5*
75
"
— 10
33 . 5 SbBr3
20
50-5
"
31 t
83-2
i.i+SbBr3
o
35-6
25
59
"
40
84.6
SbBr3
20
41.6
30-5*
77
"
60
88.4
"
40
S1^ "
30 t
77-9
"+SbBr,
[80
94.1
•
60
65
40
80.6
SbBr3
194
IOO
H
80
84
60
86.4
"
80
93-6
"
SbBr3 -f Benzaldehyde. SbBr3 -f- Benzonitrile.
SbBr3 + Benzophenone.
Gms. SbBr3 q ,. ,
•20
38.
4
i.i
-13.2'
* 0
.0 C«HBCN
48
*
0
C6HfiCO.C6H6
0
45-
5
"
-16
19
.2 "
40
24
"
20
54-
3
"
— 18 t
28
.7 "+i.i
29
t
41.
2
"+i.i
35
64.
i
"
0
43
i.i
40
50
i.i
40
70.
3
"
20
59
"
45
56,
3
"
41.
5* 77-
"
30
67
"
48
• 5
*66,
A
K
37.
8f 84.
4 i
,i+SbBr3
38*
77
.8
45
76
"
55
88
SbBr8
35 t
'82
.5 i.i+SbBr,
40
80
i.i+SbBr3
75
93.
i
"
55
87
. 5 SbBr3
. So
82,
6
SbBr3
85
96.
i
"
75
93
•3
70
88.
7
"
90
98.
2
«
85
96
•5
80
92,
A
"
94
IOO
•
90
98
•3
90
97.
3
. "
94
IOO
94
IOO
"
* m
.pt.
t Eutec.
t
tr. pt.
I.I
= compound
of equimolecular
amounts of the two constituents in each case.
ANTIMONY TriBROMIDE
RECIPROCAL SOLUBILITIES OF ANTIMONY TRIBROMIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910.)
SbBr3 +
Brombenzene.
Gms. SbBr3
t°. per 100 Gms.
Sat. Sol.
-31*
o
-32
5-7
-25 1
9-5
-15
15
— 5
20.8
+ 5
26.8
i5
33
25
39-6
45
54-6
65
71.9
85
90.7
94
roo
SbBr;
5 +
SbBr3 +
SbBr3 +
Chlorbenzene.
lodobenzene.
Fluorbenzene.
Gms. SbBr3
Gms. SbBr3
Gms. SbBr!
t°.
per 100 Gms.
Sat. Sol.
t°.
per 100 Gms.
Sat. Sol.
t°.
per 100 Gms.
Sat. Sol.
-45-2*
0
-28.6*
0
-39-
2* 0
-47 t
-40
5-2
6.8
-30.3
-32 t
7.0
14-3
-39-
-25
5t 1-3
4-3
-30
Q.6
— 20
21.6
-15
6-7
-20
12.6
— 10
27.5
+ 5
12.6
-10
16
o
33-4
25
21.8
0
20
+10
39-3
45
35-3
20
30
20
45-2
55
45-5
40
45-4
40
57-6
65
60.8
60
65.8
60
71.1
75
81.8
80
86.3
80
86.3
85
93-5
94
100
94
IOO
94
IOO
SbBr3 +
SbBr, +
SbBr3 +
SbBr3 +
p Dibrombenzene.
p Dichlorbenzene.
Nitrobenzene.
m Dinitrobenzene.
Gms. SbBr3
t°. per i oo 'Gms.
Sat. Sol.
Gms. SbBr3
t°. per 100 Gms.
Sat/ Sol.
Gms. SbBr3
t°. per loo Gms.
Sat. Sol.
Gms. SbBr3
t°. per loo Gms.
Sat. Sol.
88* o
54-5* o
6* o
90* o
85 10
51-5 14
I 22
80 29 . I
80 25.2
48. 5 t 26.5
- 4 37-4
70 50
75 39-2
55 35-9
- 9 48.4
60 63
70 52
60 43-1
-14- 5t 55-3
50 70 . 8
65 f 62.2
65 50.7
- 5 58.3
47-5 t 72
70 68.7
70 58.8
+ 5 61.5
50 73-4
75 75-3
75 67.2
25 68.6
60 78.2
80 8r.8
80 75.8
45 76.6
70 84
85 88.3
85 84.5
65 85.3
80 90.4
90 94-3
90 93-4
85 94-7
90 96 . 8
94 100
94 100
94 loo
94 loo
Molecular compounds are not formed in the above systems. The diagram
in each case consists of two arms meeting at the eutectic.
SbBr3 + Ethylbenzene. SbBr3 + Propylbenzene.
SbBr3 + p Cymene.
Gms. SbBr3 <,,. .
t°. per loo Gms. pS,olld
Sat. Sol. Phase-
Gms. SbBr3 A .. .
*•• Tssr« *•• F
Gms. SbBr3 g^
-93*
0
C8H6.C2H5
-80
i.
3 I-1
-75*
0
-93-2 t
0.4
"+i.i
-60
3-
7
-77 t
2
— 70
I
i.i
—40
9-
4
-So
6.
I
i.i
-50
2.2
"
— 20
22.
5
-30
12.
3
"
-30
4.8
"
— 10
38.
4
— 10
27
"
— 10
12
'«
- si
49
i.i+SbBr,
0
42.
3
"
+10
29.2
"
+10
53-
3 SbBr3
+5 t
51-
5
x.x+SbBit
20
46.3
M
20
57-
I
20
56
SbBr,
29 1
69.7
i.i+SbBrs
40
66.
2 "
40
64.
i
M
50
78.2
SbBr3
60
77
2
60
75
"
70
87.3
"
so
89.
8 it
80
88.
5
M
90
97-7
"
94
IOO
"
94
IOO
M
* m. pt.
t Eutec.
tr. pt.
i.i = compound of equimolecular amounts of the two constituents in each case.
ANTIMONY TriBROMIDE
86
RECIPROCAL SOLUBILITIES OF ANTIMONY TRIBROMIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1911.)
SbBr3 + Cyclohexane. SbBr3 + Pseudo Cymene. SbBr3 + Mesitylene.
Gms. SbBr3 s ,-, Gms. SbBr3 «,,.. Gms. SbBr3 <, ...
t°. per loo Gms. p>._.. t°. per 100 Gms. ^u t°. per 100 Gms. i2~
Sat. Sol. Sat. Sol. Sat. Sol. Phase'
6.4* o CsHu —57-^* o C6H3(CH3) !, 2, 4 — 54.4* o QH^CHj), i, 3, 5
6f 0.3 CeHu+SbBr, -58.8 f 9-7 " +i-i ~55-2f 2.1 " +1.1
•20 1.4 SbBr3 —50 II i.i —30 3.6 i.i
40 3.7 —30 16.2 —io 9
60 7.1 —io 31 +10 25.4 "
80 12.5 o 47.6 " 20 35. $
liquid layers formed
7§ 63.5 1.1+2.1
29 t 46.5 i.i +2.1
92.5 17.4 97.6
IS 67.4 2.1
40 54 . 2 2.1
no 25.8 96.5
25 73
50 61.7
130 36.4 95
33 § 79.1 2.i+SbBrs
60 70 . 2 "
150 47.8 92.7
50 82.8 SbBr3
69.5*85.8
170 62.3 86.3
70 88.4
69! 87.7 2.i+SbBr3
175 1 74.0
90 97.4
80 92.7 SbBr3
SbBr3 + Diphenylmethane
. SbBr3 + Naphthalene.
SbBr3 +a Nitronaphthalene.
Gms. SbBr3 g0ji(j
Gms. SbBr3 ~ ,..
t°. per loo Gms. £?™
Gms. SbBr3 Sojjd
Sat. Sol. ase'
Sat. Sol. •Fhase'
Sat. Sol. Phase.
26 * o CH2(C6H5)2
79.4* 0 ' C10H8
57* o.o aC10H7N02
22. 5 f 12.8 "+2.1
75 23.7
50 23.2
40 22.8 2.1
70 37-4
40 42.6
50 29.5
65 48.6
33-5 1 50.5 "+«
60 37-5
57 6l.2 " +2.:
t 37.5 62.6 i.ilf
70 47-8
60 68 2.1
38.2* 67.6
80 60.2
65 81.3
38 f 68 i.i+SbBr,
90 * 81 . i
66* 84.9
50 73.4 SbBr3
85 89.6
65 f 86.7 2.i+SbBr3
70 83.8
82f 92.2 2.i+SbBr3
75 90.1 SbBr3
90 96.4
90 96 . 2 SbBr3
85 94-9
94 IOO "
90 97.7
SbBr3 + Diphenyl.
SbBr3 + Phenol.
SbBr3 + Phenetol.
Gms. SbBr3 s ,. ,
t°. per loo Gms. ^,?lld
Sat. Sol. Phase-
Gms. SbBr3 c rj
*•• •isssr $£•
Gms. SbBr3 goli(j
,'70.5* o C6H6C6H5
41 * 0 C6H5OH
-28.6* o C6H6OC2H5
60 35.7
35 22.5
— 29 1 1.6 " +1.1
50 54-3
30 40
— io 4.8 i.i
47 1 57-4 "+2.1
28.5! 44-6 "+2.1
+10 12.9
55 68.5 2.1
40 53 2.1
20 19.2 "
60.5* 82.7
50 62.5
30 29.7
70 86 . S SbBr2
60 75.8
4O 46 . 2
80 91.5
65 84.7
48.8* 74-7
90 97-3
66.5* 88.5
47 1 77-8 i.i+SbBr8
94 loo
75 91 • 7 SbBr3
60 83 SbBr3
85 95-8
70 87.3
90 98.1
90 97.4
* m. pt.
t Eutec. t crit. t.
§ tr. pt.
H Not obtained regularly,
in such cases, single eutectic at
23° and 61.5 per cent SbBr3.
i.i = compound of equimolecular amounts of the two constituents in each case.
2.1 = compound of 2 molecules of SbBr3 with one molecule of the other con-
stituent.
ANTIMONY TriBROMIDE
RECIPROCAL SOLUBILITIES OF ANTIMONY TRIBROMIDE IN VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910-12.)
naphthalene.
Gms. SbBr3
per loo Gms.
Sat. Sol.
O
,3.8
22.6
27.3
35-5
46.7
61.6
69.9
78.6
87.5
96.6
IOO
SbBr3 + a Brom-
SbBr;
naphthalene.
nap
Gms. SbBr3
t°. per 100 Gms.
t°.
Sat. Sol.
3*
-17s
o 15-8
— 21
- 3-St 3i-4
— 24.
15 38.7
— IO
35 49-9
+10
45 56.9
30
55 64.7
65 72.9
g
75 81.8
70
80 86.3
80
85 90.8
90
90 95.4
94
SbBr3+/3Chlor-
naphthalene.
SbBr3 + Tetra-
hydrobenzene.
Gms. SbBr3
Gms. SbBr3
t°.
per 100 Gms.
Sat. Sol.
t°.
per 100 Gms.
Sat. Sol.
56*
O
...
50
26.1
-5
ii. 7
45
38.5
IS
40
49
35
24.1
37- St
53-6
55
41
45
58.8
65
55-1
55
66.8
70
64-5
65
75-2
75
76.2
75
83-8
80
84-4
80
88.1
85
90.7
85
92.4
90
95-8
90
96.7
94
IOO
SbBr3 +
SbBr3 +
SbBr3 +
SbBr3 +
o Chlortoluene.
m Chlortoluene.
p Chlortoluene.
m Nitroluene.
Gms. SbBr3
Gms. SbBr3
Gms. SbBr3
Gms. SbBr3
t°.
per loo Gms.
Sat. Sol.
t°.
per 100 Gms.
Sat. Sol.
t°
per loo Gms.
Sat. Sol.
tv,
i
per 100 Gms.
Sat. Sol.
-36,
2* 0
-47-8*
0
6
.2* 0
16*
0
-38.
St i°-7
-50 t
8.1
2
•St 23.3
10
24.2
— 20
15-4
-30
IX .7
2O
33
5
39
0
22.S
— io
17.5
30
39-3
o
46.6
+ 20
32.5
+ 10
25.8
40
47-2
- 9t
56.8
30
38.8
30
37-5
50
56.3
+10
62.7
40
46.8
40
45-1
60
66.7
30
69.7
50
60
56
66.5
£
54-4
65
70
80
77-8
88.2
f
60
77-5
8i-S
g
77-8
88.2
70
80
77
88.2
90
94
97
IOO
70
80
86.3
91.4
90
97
90
97
90
97-2
Molecular compounds are not formed in the above systems. The diagram in
each case consists of two arms meeting at the eutectic.
SbBr3 + Toluene. SbBr3 + o Nitrotoluene.
Gms SbBr3 Solid
SbBr3 + p Nitrotoluene.
Gms. SbBrj «, ...
Sat. Sol.
5at. Sol
rnase.j
Sat. So
-93*
0
C6H5.CH3
- 8.5*
O
o N02.C6H4.CH3
52-5*
0
-93-5t
I.O
"+i.i
-13-5
19-5
" +1.1
45
29.8
-80
2.4
i.i
O
27.6
i.i
40
42.2
-60
6.2
"
IO
35-6
"
35
50
—40
12.4
"
20
47-5
"
25
61
— 20
25-7
"
25
55-7
H
i6f
67
- It
53.1
1. 1+2. 1
31 t
70
" +SbBr3
30
71.6
+ 20
30 t
69.4
78
2.1
2.i+SbBr3
40
5°
73-5
77-5
SbBr3
g
78.9
82.9
40
80.6
SbBr3
60
81.7
•
70
87.2
60
86.6
•«
80
91.4
"
80
92
80
93-8
"
90
97-2
"
90
97-5
94
IOO
"
P N02.C6H4.CH3
+SbBr,
SbBr3
* m. pt.
t Eutec.
tr. pt.
i.i = compound of equimolecular amounts of the two constituents in each case.
2.1 = compound of 2 molecules of SbBr3 with i molecule of the other con-
stituent.
ANTIMONY TriBROMIDE 88
RECIPROCAL SOLUBILITIES OF ANTIMONY TRIBROMIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910-11.)
phe^y?mtt£iie. SbBr3 + o Xylene. SbBr3 + m Xylene. SbBr3 + p Xylene.
Gms. SbBrs
t°. per 100 Gms.
Sat. Sol.
Gms. SbBr3
t°. per 100 Gms.
. ' Sat. Sol.
Gms. SbBr3
t°. per loo Gms.
Sat. Sol.
Gms. SbBr3
t°. per 100 Gms.
Sat. Sol.
92*
0
-29*
O
-57*
o
14*
o
85
18
-33 t
10-5
-59- 2 t
5-5
12
16.6
80
30.1
— 20
17
-45
10
lot
28
70
47
— 10
24.6
-35
14.2
2O
36
00
48 1
58.2
67.1
0
2O
34-5
65.8
-25
- 5
20
38.8
30
40
44-6
53-8
60
70
73-3
79-5
24*
22. St
77.2
78.6
+ 5
12.5 $
56.6
75-4
t
63-5
74
80
86.4
30
80
25
77-6
67-5*
87.3
90
95-2
50
84.7
45
82.3
66. st
88.3
94
100
70
90.1
65
87.9
75
91.4
90
97-7
87
95-3
85
95-7
* m. pt. f Eutec. J tr. pt.
In the case of each of the above xylenes the compound existing between the
first and second eutectic consists of equimolecular amounts of SbBr3 and xylene.
Solubility data determined by the freezing-point method (see footnote, page i)
are given for mixtures of antimony tribromide and each of the following compounds :
azobenzene, benzil, s diphenylethane and stilbene (Van Stone, 1914), aniline, ben-
zophenone, triphenylmethane and toluene. (Kurakov, Krotkov and Oksman, 1915.)
ANTIMONY TriCHLORIDE SbCl3.
SOLUBILITY IN WATER. SOLID PHASE SbCl8.
(Meerburg — Z. anorg. Chem. 33, 299, 1003.)
Mols. SbCU Gms. SbCla Mols. SbCla Gms. SbCl3
t°. per loo per 100 t°. per 100 per 100
Mols. H2O. g. H2O. Mols. H2O. g. H2O.
o 47.9 601.6 35 91.6 1152.0
15 64.9 815.8 40 108.8 1368.0
(72.4 9IO-I 50 152.5 1917.0
(74-1 931.5 60 360.4 4531-0
25 78.6 988.1 72 oo oo
30 84.9 1068. o
SOLUBILITY OP ANTIMONY TRICHLORIDE IN AQUEOUS HYDROCHLORIC
ACID. SOLID PHASE SbCl3. TEMP. 20°.
(Meerburg.)
Mols. per
100 Mob. H2O.
Gms
100 g
:Sb.
Mols. per
100 Mols. H2O.
Gms. per
100 g. H2O.
HC1.
0
2.4
6.1
8-3
SbCla.
72.4
71.2
69.9
68.2
HC1.
o.o
4-86
12-34
16.80
SbCla.
910.1
895-4
879.0
857.6
HC1.
9.1
II-7
28.7
SbCl3'.
68.9
68.1
62.8
HC1.
18.41
23.68
58.08
SbCla.
866.4
856.3
789.8
loo gms. absolute acetone dissolve 537.6 gms. SbCla at 18°. d*p sat. sol. = 2.216.
(Naumann, 1904.)
loo gms. ethyl acetate dissolve 5.9 gms. SbCl3 at 18° d sat. sol. = 1.7968.
(Naumann, 1910.)
89 ANTIMONY TriCHLORIDE
RECIPROCAL SOLUBILITIES OF ANTIMONY TRICHLORIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1911.)
SbCl3 + Acetic Acid. SbCl3 + Acetophenone. SbCl3 + Anisol.
Gms. SbCl3 o-,, Gms. SbCl3 S,;H Gms. SbCl,
16.5* o
10 22.7
o 42.5
- 5 48.5
- 9t 52.7
o 59
CH3COOH 19 . 5
IS
ft
" +1.1 IS
i.i 35
*
o C6H6COCH3 -34*
14-3 -36.5
28.5 -30
31.8 '• +1.1 —io
35-4. LI +10
41.6 20
t
0
n. 8
16
28.3
43
52.8
C«H6OCH3
" +1.1
i.i
IO
67.3
55
55
.2
"
251
63.6
" +2.1
19*
"79.1
60.5
*
65
4
"
35
70
2.1
25
81.5
SbCl, 45
79
3
"
41-5
*
80.9
"
45
87.4
32 t
84
i.i+SbCl,
40 t
84-5
"+SbCl3
65
95-3
So
89
3
SbCl3
60
.92
SbCl3
73
IOO
70
98
,2
70
98
SbCl3 + Aniline.
SbCl3 + Benzaldehyde.
SbCl3
+- Benzophenone.
Gms. SbCl3 g ,5. Gms. SbCl3 Solid
Gms. SbCl3 o ,. ,
t°. per too Gms. T>I ' t°. per ioo Gms. pv,00 t°. per ioo Gms. pu^
c«4- c.r.1 jrnase. GO+- c^i iiio.sc. Qot Q/^I x ua,»c.
t x
C6H5NH2+i.4
IO
43
. 5 x.i
48
*
o
C8H5COC,H5
+ 20 '2
7
1.4
20
47
• 5
40
16.3
"
60
18.
7
"
30
52
• 4
35
t
21.6
" +1.1
77 t
29.
6
I-4+I-3
40
60
.2
45
26.2
i.i
88*
44-
8
1-3
43
• 5*
68
. I "
55
31-4
"
87 t
46.
3
1.3+1-2
40
74
.2 "
65
37-5
"
94-5* 54-
9
1.2
30
80
.6
76
*
55-4
"
89-5
61.
7
1. 2+1. 1
25
t
83
i.i+SbCl3
65
71.6
"
100.5
* 71
I.I
35
85
SbCl3
45
80.6
it
70
82.
2
"
45
87
•5
39
t
82.7
"+SbCl3
3i t
88
i.i+SbCl3
65
95
.2
50
87
SbCl3
60
94-
9
SbCl3
73
IOO
"
70
97-7
"
i.i = compound of equimolecular amounts of the two constituents in each case.
2.1 = compound of 2 molecules of SbCl3 with i molecule of the other constit-
uent.
1.2, 1.3 and 1.4 = compounds of i molecule of SbCl3 with 2, 3 and 4 molecules
of aniline.
SbCl3 + Benzoic
Acid.
SbCl3 + Benzoyl
Chloride.
SbCl3 +- Benzene
Sulphonic Acid.
SbCl3 + Tetra-
hydrobenzene.
Gms. SbCl3
'Gms. SbCl3
Gms. SbCl3
Gms. SbCl3
t°.
per ioo Gms.
Sat. Sol.
t°
per ioo Gms.
Sat. Sol.
t°.
per ioo Gms.
Sat. Sol.
t°.
per ioo Gms.
Sat. Sol.
1 20
O
- 5
I7.8
52-5*
O
-25
19.1
no
23
-IS
36.8
45
18
-15
24
IOO
38.8
-23 t
45
25
43-7
- 5
30
90
50
— 5
5°- 7
5
56.i
+ 5
37- *
80
59
+15
58.2
-5t
60.8
IS
45-1
70
66
25
62.9
+5
49-8
25
54-3
60
71.6
35
68.4
25
56.7-
35
64.5
46 1
78
45
74-9
45
69.2
45
74
60
89.2
55
82.4
65
90.2
55
83.6
70
97-5
70
96.5
73
65
92.8
Molecular compounds are not formed in the above systems. The diagram in
each case consists of two arms meeting at the eutectic.
* m. pt.
t Eutec.
I tr. pt.
ANTIMONY TriCHLORIDE
90
RECIPROCAL SOLUBILITIES OF ANTIMONY TRICHLORIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, igio-'n.)
SbCl3 + Benzene. SbCl3 + Brombenzene. SbCl3 + Chlorbenzene.
Gms. SbCl, <^,.,1 Gms. SbCl, <,,.. Gms. SbCl, -...
4*
7-3
QH, .
-3i t
0
C«H6Br
-45
.2f 0
QH5C1
i
19.4
" +2.1
-32-5*
4.8
" +1.1
-47
4-3
" +1.1
10
24.6
2.1
-30
6.8
i.i
-40
7
i.i
20
30.5
"
— 20
14.8
"
-30
ii. i
40
44.1
"
— io
23-9
"
-IS
20.5
60
60.6
H
o
34-3
H
- 5
32.5
79 t
£5
«
«
+ 3t
20
40-3
52
i.i+SbCl,
SbCl,
o
20
t 44-2
56
70
93-5
"
40
68
"
40
72.1
62*
96
2.1+SbCl,
60
85.8
II
60
88.2
67.5
97-9
SbCl,
73
IQO
II
73
100
SbCl3 + Fluorbenzene.
SbCl3
+ lodobenzene.
SbCl3 + Nitrobenzene.
Gms. SbCl, g^ Gms. SbCl, Solid Gms. SbCl, Solid
-39.2
t o
QHjF
-28. 6f
Sat. Sol.
0
C«H5I
6f o
CANO,
-40-5
* 2.4
"+ i.i
-35 ^
12.8
"
— 2
20.4
1
-25
II
i.i
-45*
29.8
"+i.i
— 10
* 32
M
-IS
17.3
"
-34-5
11.7
i.i, unstable
-16
•5* 38
" +I.I
— 10
21.4
"
-IS
26.4
(i «
— io
5 44
I.I
- 5
26.4
"
- 3
. 49 • i
" "
- 7
5 So
ii
0
34.1
"
-35
32.5
i.i+SbCl,
- 6
t 64.8
1C
+ 5-5
t 45.8
i.i+SbCl,
-IS
38.9
SbCl,
- 6
5* 67.5
i.i+SbCls
15
53.6
SbCl,
+ 5
46.4
"
+ 5
69.6
SbCl,
25
61.6
"
25
56
<i
35
78.7
"
45
77.7
«
45
69.6
«
55
87.4
"
93.8
«
65
88.8
<<
70
96.6
"
SbCl3
+ Ethylbenzene.
SbCl3
+ Benzonitrile.
SbCl
3 + Isoamylbenzene.
Gms. SbCl, C^I.M Gms. SbCl, ^.j
Gms. SbCl,
t°.
per 100 Grr
MMBU
t .
Der zoo G
ms. p]ko
t .
per 100 Gms
Ph
Sat. Sol.
Sat. So
L
Sat. Sol.
-93 t
0
QHs-QHs
— 13.2 f
0
QHsCN
-80
4
I.I
-93-5
* 0.3
" +1.1
-16
IO.2
"
-60
11.7
"
-70
0.6
i.i
-19*
17.2
" +1.1
—40
25-4
«
-50
i.i
— 10
21.9
i.i
-33
t 32.7
1. 1+2. 1
-30
2.5
0
28.5
-25
38.7
2.1
— 10
7
10
38.7
-15
47-2
"
+ 10
18.8
15
47.4
- 5
t 56.8
2.i+SbCl,
30
44-4
20
62.6
o
57-4
SbCl,
39 t
68.1
21. 5t
68.7
20
63.3
"
35*
77-4
I.I+2.I
20
72.4
40
72.6
«<
37 t
81.1
2.1
IS*
78.9
60
.87.1
«<
36.8
* 81.8
2.1+SbCl,
25
81.6
70
97.3
ii
So
87.2
SbCl,
45
87.6
70
98
"
65
95-6
-25
44.4 unstable i.i
73
— 21
t 54-9
"i.i+SbCl,
33
8o.*4
i.i+SbCl,
(unstable)
— IO
56
"SbCl,
Eutec.
t m. pt.
t tr. pt.
i.i = compound of equimolecular amounts of the two constituents in each case.
2.1 = compound of 2 molecules of SbCl3 with i molecule of the other con-
stituent.
ANTIMONY TriCHLORIDE
RECIPROCAL SOLUBILITIES OF ANTIMONY TRICHLORIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910-11.)
SbCl3 + m Dinitrobenzene. SbCl3 + Propylbenzene.
Gms. SbCl3 <.,..,, Gms. SbCl3 «^HH Gms. SbCl,
90*
O m CeH4(NO
2)3 20
72. 8 unstable i.i —70 O.6 2.1
80
18.6
IS
76.2 " " —30 10. 1
70
31-3
10
78.6 " " — 10 26.6 "
60
40.7
5
80.8 " " o 40.4 "
5°
48
o
82.7 " « 7 57.5
40
53-6
— IO
64.9 '• SbCl3 8. si 68.2 "+SbCl,
30
58
+ IO
69 " " 20 71.4 SbCls
20
61.6 unstable "
20
71.6 " " 40 78.5
IO
64.5 "
30
74.8 " 65 92.5
it
66 . 8 " " +SbCl3 40
78.7 "
— ii
68.8 "
50
83.5 " — 70 1. 5 i.i unstable
+27-S
52-5 " 1.1
60
89 " —30 16
28.5*
58.2
70
96.4 " - 5 48.2 "
27-5
63
73
ioo " + 1.5* 65.3 "
25
67.5
it 66.3 "+SbCl3 "
10 68.6 SbCU "
^3b<
ben
p Dichlor- SbCl3 + Cyclohexane.
zcric*
t°.
Gms. SbCl3
per ioo Gms.
Sat. Sol.
t°.
Gms. SbCls Gms Sbcj3 pg,. I00 Gmg
Sat^Sol ' Sat> S°l
88*
0
54-5*.
0 6.4* 0.0
85
5-7
So
14 6f 0.2
80
15-4
45
30 20 1.2
70
35
40
48 40 4-2
60
52.8
39-5 t
50.5 60 9.7
55
59
45
59 . 5 Two liquid layers formed
49- 5 t
64
So
67.8 70 13.7 97
65
71.8
55
75-7 80 19.5 96.1
60
79-3
60
83 ioo 32.3 92.7
70
95
70
96.2 120 57.1 83.2
124 58.9 76.7
125. 5 § 68
SbCl
3 + P Cymene,
SbCl3 + Pseudocymene. SbCl3 + Diphenyl.
Gms. SbCl3 ^r.A
Gms. SbCl3 Solid Gms. SbCl3 Solid
.*.'• P*
* too Gms. phase
t°.
Per ioo Gms. phase *°. ^c^Sol118' Phase-
-75*
0 P C6H4CH3C3H7
—57.4
* o C6H3(CH3)3l,2,4 70.5* 0 QH5.QH,
-76. st
2 " -{-I.I
-6ot
18.6 " +1.1 65 14
-So
7 i-i
-45
23.6 i.i 55 33-4
-30
IS
-25
33-3 sot 40 "+2.1
— IO
30
— IO
45 55 45-2 2.1
-.3. si
41 I.I+2.I
- si
50.7 " +2.1 60 51.4
10
46.1 2.1
+15
55.8 2.! 70 70.7
30
60
35
62.2 " 71* 74-6
40 i
76.4 2.I-fSbCl»
So
69.7 " 65 85.5
So
81.2
56*
79.2 " 57 1 88.9 2.1+SbCl,
60
87
Sit
87.5 2.i+SbCl3 65 93.1 SbCl,
70
95-6
65
93.9 SbCl, 70 97
* m. pt.
t Eutec.
tr. pt.
§ crit. t.
i.i = compound of equimolecular amounts of the two constituents in each case.
2.1 = compound of 2 molecules of SbCl3 with I molecule of the other constituent.
ANTIMONY TriCHLORIDE
92
RECIPROCAL SOLUBILITIES OF ANTIMONY TRICHLORIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910-11.)
SbCl3 + Mesitylene.
Cms. SbCl3
Cms. SbCl3 oni;j
SbCl3 + Triphenyl
Methane.
Cms. SbClj o 1; ,
— 54-4 o CgHs(CH^3i,
3,5 26*
o
CHZ(C6H5)2
92*
o
CH(C6H6)3
-55-6
i.
5
" +1
i 22.5'
t 7-9
" +2.!
85
ii. 8
"
-40
3
I.I
40
15.1
2.1
80
19-3
"
— 20
7
«
60
26
«
70
32
"
0
14.2
(i
70
33
60
42.4
"
10
20.
3
«
80
41.6
So
49-6
««
3°
39-
3
"
9°
52-7
49 t
5°
" +1.1
f*
65
£:
4
4
2.1
1 9S*
100*
59-8
72.9
45
40
62.8
68.3
i.i
75-5* 79-
2
"
95
82.2
35$
72
i.i+SbCl3
70
87
"
90
86.7
45
76.6
SbCl3
58.5
92.
4
" +SbCl3 80
91-5
55
82.4
««
63
94
SbCl3
67 I
95-7
*.
i+SbC!3
65
90.6
«
70
98
"
70
97
SbCl?
70
96.1
"
SbCU
+ Naphthalene. ^naphthalene?1'"
SbCl8 + 18 Chlor-
naphthalene.
Cms. SbCl3 c vj Gms. SbCl3 Solid Gms. SbCl3 g i- j
t°. per i oo Gms. pv,oca t°. pe^ioo Gms. pv..^,, t°. per 100 Gms. pv,oco
I79-4*
Sat.
o
sol.
C10H8
i
-17*
0
a CioH7Cl
56
£
at. Sol
0
0 C10H7C1
75 .
IS
.2
M
— 21 t
8.1
" +2.1
5°
16.6
"
.65
35
"
O
14.4
2.1
45
27.2
"
59 t
42
.8
" +2.1
IO
18.7
"
40
35-4
"
65
48
•4
2.1
20
24.6
ii
30 A
47-3
*
75
58
.8
"
30
33-5
"
25 t
52-3
" +1.1
80
65
"
40
47-7
"
29-5*
58.2
i.i
86*
78
"
45
61.5
"
28 1
64
i.i+SbCl,
80
88
•7
«'
46*
73-6
"
35
68.3
SbCl3
70
93
*
45-5 J
75
2.1+SbCla
45
75-3
»
65 J
94
2.1+SbCl,
55
82.2
SbCl3
60
87.5
"
70
97
.2
SbCl3
70
90-5
73
I
00
"
SbCl3 + a
Bromnaphthalene.
SbCl3 +
a Nitronaphthalene.
t°.
Gms. SbCl3 per 100
Gms. Sat. Sol.
Solid
Phase.
t°
Gms. SbCl3 per 100
Gms. Sat. Sol.
Solid
Phase.
3*
o
a CwH7Br
57
*
0
a C10H7N02
- it
8-3
" +1.1
50
13
.6
•
"
10
12.8
i.i
40
27
•3
"
25
• 24
"
30
t
35
.8
" +1.1
33
38.5
"
35
43
.2
i.i
34-5
*
52.4
"
37
•5
49
•3
"
33
62.1
«<
39
*
56
•7
"
31.5
t
64.7
i.i+SbCl3
37
•5
64
"
40
69.7
SbClj
34
i.St
72
.8
i.i+SbCla
£
76.2
84.5
«.
45
60
78
87
•4
SbCl3
70
94-8
"
70
96
.6
"
" m pt. t tr. pt. t Eutec.
i.i = compound of equimolecular amounts of the two constituents in each
case.
2.1 = compound of 2 molecules of SbCl8 with I molecule of the other con-
stituent.
93'
ANTIMONY TriCHLORIDE
RECIPROCAL SOLUBILITIES OF ANTIMONY TRICHLORIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910-12.)
SbCl3 + Phenol.
Gms. SbCl, o-ijj
SbCl3 + Phenetol.
Gms. SbCl3 o,..
SbCl3 + Toluene.
Gms. SbCl3 o^i:-i
t°. per zoo Gms. £?** t°. per !oo Gms. fT"™ t°. per 100 Gms. pT"t
Sat. Sol. ££se' , Sat. Sol. Sat. Sol.
41*
0
C6HBOH
-28
.6*
O
1"* TT r\(~* T3
[5 -93
*
0
C,H6.CH3
35
16.2
"
-29
t
I
• 4 "+!•
i -94
t
i
.1
" +i.l
30
25.6
"
— 20
4
.5 I.I
— 70
3
. i
i.i
20
38.7
"
— 10
8
.1
-30
IS
.8
"
10
48
Cl
+ 10
18
.2
O
•5
"
St
52
" +3.1
2O
27
4
II
I
57
.8
" +2.1
IS
58.6
2.1
30
39
.4
20
62
.8
2.1
30
70.6
"
40
58
"
40
78
"
37*
83 -
"
42
.2*
65
"
42
•5*
83
. i
"
36. 5 t
83.7
2.I+SbCl3
35
t
77
.8
40 t
85
.8
2.i+SbCl3
55
90.6
SbCls
So
86
8
50
89
SbCl3
70
98.2
H
70
97
i
70
97
.8
"
SbCl3 + o Chlortoluene. SbCl8 +\m Chlortoluene.
I
to
ims. SDI
nS Solid
Li
rmS. 3D
pe
r 100 Gi
ns- Phase.
t°.' pe
r 100 G
-36.2*
O
o C1C6H4CH3
-47-8*
0
-37- St
6.9
" +1.1
-49 t
6.9
— 20
I8.3
i.i
—40
12.3
— 10
29.2
"
-30.
20.1
- 5
37-i
"
— 20
31
- o.st
47-9
i.i+SbCl3
— 14 1
40
+ 10
SbCl3
o
46.!
20
5^2
M
10
51.6
3°
64.6
M
20
57-4
40
71.8
II
40
72.8
60
88.4
"
60
89.1
+1.1
SbCl3
- 7-St
73
73
IOO
o
10
30
40
50
60
70
o
12.7
23-5
32.2
43-8
47-2
52.2
64.8
72-3
80.2
88.8
97-4
SbCl3 + p Chlortoluene.
Gms. SbCl3 c ...
6.2
3
o
3
7
'+SbCl3
SbCl3 + o Nitrotoluene. SbClg + m Nitrotoluene. SbCl3 + p Nitrotoluene.
Gms. SbCl3 ' Sol.
, . [Gms. SbCl3 g.
Gms. SbCl3 q ...
t°. per loo Gms. ^
J. t°. per toe Gms. ,$£
se t°.
>er 100 Gms. pi?
Sat. Sol. ,Fha
>e- Sat. Sol.
Sat. Sol. *flase'
-8.5* 0 oNOsQ
H4CH3 16* 0 wNOjC
^CHs 52.5
* o p NOzQ^CH
-13-5 II- 3
io 15
45
18.5
-iS.st 18.5
+n o 30.7
35
33-6
— io 21.3 i.
i —io 39.2
30 '
38.8 "
+ 10 31.1
— 20 42.8
1 20
46
20 39
crystallization not
7-5
t 52 " +i.x
30 So
obtained here
7-5
* 62.3
34-5 * 62.3
o 67 . 2 Sb
Cl, 5
66.1
33 68
20 72.5
3t
68.5 i.i+SbClj
27- St 74-6
+SbCl3 30 76.3
10
70 SbCU
40 79 . i Sbl
:i, 40 80.8
30
^75-5
50 84-5 *
50 86
So
85
70 97-5
1 60 91.6
70
97-5
73 loo
t Eutec.
t tr. pt.
• m. pt.
i.i = compound of equimolecular amounts of the two constituents in each
case.
2.1 = compound of 2 molecules of SbCl8 with i molecule ot the other con-
stituent.
ANTIMONY TriCHLORIDE
94
RECIPROCAL SOLUBILITIES OF ANTIMONY TRICHLORIDE AND VARIOUS ORGANIC
COMPOUNDS, DETERMINED BY THE "SYNTHETIC METHOD."
(Menschutkin, 1910.)
SbCl3 + o Xylene.
SbCl3 + m Xylene.
SbCI3 + p Xylene.
Cms. SbCls Solid
t°. per 100 Gms. -pi t°. p
Sat. Sol. Phase'
Gms.
SbCls Solid GmS' SbC13 Snlirl
' Gms' Phase *°- Per I0° Gms- PI?
Sol. Phase' Sat. Sol. Phase. _
•29.
0
0C6H4(CH3)2 -57*
O
7W L-c-H-4 (0.11.3)2 14
*
0
P C6H4(CH3)2
•35
t 14
" +1.1 —60.5
t 7
•5
" +I.I II
•71
1" Ir
• 7
"
+I.I
30
17-
5
™ —45
15
.8
I.I 2O
i7
•5
i.i
•20
24.
8
-25
29
40
37
•3
"
10
33-
4
— 5
46
. 2
So
52
•3
««
o
43-
4
- aj
49
.8
" +2.1 55
t
62
• 7
«•
+2.1
IO
55
5
53
.1
2.1 60
66
.1
2.1
19.
5*68.
i
IS
58
•7
70
*
81
25
71-
3
2.1 25
65
•7
6S
88
.1
"
30
75.
7
33
73
.8
58
t
92
11
+SbCl3
33.
5 * 81
38*
81
69
97
. 2
SbCl3
5t82.
5
2.i+SbCl3 36.5
t 83
, 7
2.I+SbCl3
m
5°
88
SbCl3 50
87
•7
SbCl3 10
20
• 7
P C6H4(CH3)2 unstable
60
92.
4
60
91
5
" 7
t
32
.8
"k+2.
1
71
98.
5
70
97
,2
35
50
•3
2.1
•«
55
62
•7
"
*
* m. pt.
t Eutec.
t tr. pt.
i.i = compound of equimolecular amounts of the two constituents in each case.
2.1 = compound of 2 molecules of SbCl3 with i molecule of the other con-
stituent.
DISTRIBUTION OF ANTIMONY TRI AND PENTACHLORIDES BETWEEN AQUEOUS
HC1 AND ETHER AT ROOM TEMPERATURE
(Mylius, 1911 )
When i gm. of antimony as SbCl3 or as SbCl5 is dissolved in 100 cc. of aq.
HC1 of the following strengths and the solution shaken with 100 cc. of ether,
an amount of metal, depending upon the concentration of the aq. acid solution,
enters the ethereal layer.
With i% SbCl3 Solution.
Per cent Cone. Per cent of Total
of HC1. Sb in Ether Layer.
With i %SbCl6 Solution.
20
15
10
S
i
6
13
22
8
0-3
Per cent Cone,
of HC1.
Per cent of Total
Sb in Ether Layer.
20
81
15
10
22
6
5
i
2-5
trace
Solubility data determined by the freezing-point method (see footnote, p. i)
are given for mixtures of antimony trichloride and each of the following com-
pounds: azobenzene, benzil, s diphenylethane, and stilbene (Van Stone, 1914);
benzene, naphthalene, diphenylmethane and triphenylmethane (Kurnakov,
Krotkov and Oksman, 1915); SbBr3, SbI3, and SbBr3 + SbI3 (Bernadis, 1912);
SbCU (Aten, 1909).
ANTIMONY PentaCHLORIDE SbCl6.
Data for the freezing-points of mixtures of antimony pentachloride and anti-
mony pentafluoride are given by Ruff (1909).
95 ANTIMONY TriFLUORIDE
ANTIMONY TriFLUORIDE SbF3.
SOLUBILITY IN WATER.
(Rosenheim and Grunbaum, 1909.)
Gms. SbF3 per 100 Gms.
O
2O
22.5
25
30
SOLUBILITY IN AQUEOUS SOLUTIONS OF SALTS AND OF HYDROFLUORIC ACID AT o°.
Normality Gms. SbF3 per 100 Gms. H2O present in Aq. Solutions of:
Water.
Sat. Solution.
384.7
79-4
444-7
8l.6
452.8
81.9
492.4
83.1
563.6
84.9
Solution. KC1. KBr. KNO3. K2SO4. K2C2O4. (NH^CA- K2C4H4O6. HF.
4 I 461.8 448.7 458.2 419.9 465.7 ... 461.4 432.5
0.5 448-3 45° 45J-9 408.5 481.2 431.9 430.5 404
0.25 431.9 455-6 418.3 406.6 451.3 442.3 430.8
o 125 407.3 417-2 401.4 ... 405-2 433-3 435-2 *479-4
* (2 n HF.)
Celluloid flasks were used and all measuring apparatus provided with HF re-
sistant coating. The SbF3 was prepared in the form of rhombic transparent
crystals from Sb2O3 and HF.
ANTIMONY TrilODIDE SbI3.
SOLUBILITY IN METHYLENE IODIDE AT 12°.
(Retgers, 1893.)
loo parts CH2l2 dissolve 11.3 parts SbI3. Sp. Gr. of solution = 3.453.
SOLUBILITY DATA DETERMINED BY THE FREEZING-POINT METHOD ARE GIVEN
FOR MIXTURES OF:
Antimony triiodide and arsenic triiodide.
(Quercigh, 1912; Jaeger and Dornbosch, 1912; Vasilev, 1912.)
phosphorus triiodide. Qaeger and Dornbosch, 1912.)
iodine. (Quercigh, 1912.)
ANTIMONY TriOXIDE Sb2O3.
Freezing-point data are given for mixtures of antimony trioxide and antimony
trisulfide. (Quercigh, 1912.)
ANTIMONY TriPHENYL Sb(C6H6)3.
Freezing-point data are given for mixtures of antimony triphenyl and mercury
diphenyl and for antimony triphenyl and tin tetraphenyl. (Cambi, 1912.)
ANTIMONY SELENIDES SbSe, Sb2Se.
Freezing-point data for SbSe + Ag2Se and Sb2Se + AgSe. (Pglabon, 1908.)
ANTIMONY TriSULPHIDE Sb2S3.
looo cc. water dissolve 0.00175 gm. Sb2S3 at 18°. (Weigel, 1907.)
SOLUBILITY DATA DETERMINED BY THE FREEZING-POINT METHOD ARE GIVEN
FOR MIXTURES OF:
Antimony trisulphide and cuprous sulfide. (Parravano and Cesaris, 1912.)
stannous sulfide. " "
lead sulfide. (Jaeger and Van Klooster, 1912; Pe*labon, 1913.)
" " " silver sulfide. (Jaeger and Van Klooster, 1912,)
ANTIMONY TARTRATE
96
ANTIMONY Potassium TARTRATE C2H2(OH)2(COOK)(COOSbOUH2O.
loo gms. water dissolve 5.9 gms. salt at room temp. (Squire and Caines, 1905.)
6.9 " " " 25°. (S and S. 1903.)
" " " 8 " " " 21°. (Aschan, 1913.)
" 95% HCOOH dissolve 82.7 gms. salt at 20.8°. (Aschan, 1913.)
" glycerol dissolve 5.5 gms. salt at 15.5°.
SOLUBILITY OF ANTIMONY POTASSIUM TARTRATE IN AQ. ALCOHOL
SOLUTIONS AT 25°.
(Seidell, 1910.)
Wt. Per cent
QH6OH in
. t Gms. C4H4O«.
Sat Sol KSbO.|H2Oper
Sat. bol. IOQ Qms gat Sol
Wt. Per cent
C2H5OH in
Solvent.
<*25 Of
Sat. Sol. l
Gms. C4H4O6.
KSbO.*H2O per
0
I.O52
7^5
40
o-935
0.38
5
1.025
5-50
50
0.913
0.23
10
1.007
3-92
60
0.890
0.12
20
0.980
I. Q2
70
0.866
0.06
30
0.958
0.84
IOO
0.788
trace
ANTIPYRINE CUH12N2O.
IOO gms. water dissolve 80 gms. CnHi2N2O at 15°. (Greenish and Smith, '03.)
"
IOO
*
alcohol
" IOO
90% alcohol
' 75-2
chloroform
1 IOO
;
ether
1.3
pyridine
50% aq. pyridine
1 38.0
1 79.61
«
25
at 20-25'
(U. S. P.)
(Enell, 1899.)
(Dehn, 1917.)
THE SOLIDIFICATION POINTS OF MIXTURES OF ANTIPYRINE AND CHLORAL
HYDRATE.
(Tsakalatos, 1913.)
toof
Solidification.
Gms.
108.9
90
70
50 . 5 Eutec.
60
62.3 m. pt.
60
56 Eutec.
IOO
86.1
73
64.2
56.8
53-2
50-3
47.2
Solid
Phase.
CUH12N20
"+i.a
to of Gms. CUH12N20 SnllM
Solidification. f
>er zoo urns
Mixture.
Phase.
60
61.8 m. pt.
40.9
36.7
1.2
it
57
So
30.1
26.1
it
40
33. 8 Eutec.
40
5i.6
20.2
I6.5
6
0
i.2+CCl3.COH.H20
CC13.COH.H,0
I.I
1.2
CUH12N2O.CC13COH.H2O (Hypnal).
CnHi2N2O.2(CCl3.COH.H2O)'(Bihypnal).
THE SOLIDIFICATION POINTS (Solubility, see footnote, p.
' ANTIPYRINE AND SALOL.
(Bellucci, 1912, 1913.)
i), OF MIXTURES OF
Initial t° of Gms' C"H,2N2O
Initial t° of Gm?' C"
Solidification.
per zoo L»ms.
Mixture.
Solidification.
112. 6
IOO
65
40
104.5
90
53
30
98
80
30 Eutec.
i7
91
70
34
20
83
60
35
10
75
50
42
0
97 APOMORPHINE HTDROCHLORIDE
APOMORPHINE HYDROCHLORIDE Ci7H17NO2.HCl.
100 gms. water dissolve 1.7 gms. salt at 15° and 2 gms. at 25°.
100 gms. 90% alcohol dissolve 2 gms. salt at 25°.
(Dott, 1906; Squires and Caines, 1905.)
ARACHIDIC ACID C20H4oO2.
SOLUBILITY DATA DETERMINED BY THE FREEZING-POINT METHOD ARE
GIVEN BY MEYER, BROD AND SOYKA (1913), FOR MIXTURES OF:
Arachidic and Stearic Acids.
Palmitic Acids.
' Lignoceric Acids.
ARBUTIN Ci2Hi607.£H2O.
100 gms. trichlorethylene dissolve o.on gm. arbutin at 15°.
(Wester and Bruins, 1914.)
ARGON, A.
SOLUBILITY IN WATER.
(Estreicher — Z. physik. Chem. 31, 184, '99.)
to Cor. Bar.
Vol. Vol. Absorbed
Absorption Coefficients.*
Solubility.
Pressure.
HaO.
Argon.
a.
/.
0.
0
.
.
0-0578
0
.0102
I
764
•9
77
.40
4
•34
0
.0561
0-0561
O
.0099
5
765
•o
77
•39
3
.92
O
.0507
0-0508
O
.0090
10
765
•3
77
.41
3
•49
o
.0450
0-0453
0
.0079
15
762
•4
77
.46
3
•13
0
.O4O4
O.O4IO
0
.0072
20
757
.6
77
•53
2
.86
o
.0369
0.0379
O
.0066
25
766
•7
77
.62
2
.64
o
•0339
0.0347
O
.0060
30
760
.6
77
•73
2
•43
0
.0312
0.0326
0.0056
35
757
.1
77
.86
2
.24
o
.0288
0.0305
O
.O052
40
758
•3
77
•99
2
.07
o
.0265
0.0286
O
.0048
45
756
•4
78
•15
I
.92
0
.0246
0.0273
0
.0045
5°
747
.6
78
•31
I
•73
o
.0221
0.0257
o
.0041
a = under barometric pressure minus tension of H2O vapor.
/ = under 760 mm. pressure.
q = grams argon per 100 g.H2O when total pressure is equal to 760 mm.
* See Acetylene, page 16.
SOLUBILITY OF ARGON AND WATER.
(von Antropoff, 1909-10.)
O
10
20
30
40
50
Coef . of Absorption.
0.0561
0.0438
0.0379
0.0348
0.0338
0-0343
The coef . of absorption adopted for these results is that of Bunsen as modified
by Kuenen. The modification consists in substituting unit of mass in place of
unit of volume of water in the formula.
Data for the solubility of argon in water and in sea water, together with a
critical discussion of the literature, are given by Coste (1917).
Data for the solubility and diffusion of argon in solid and liquid metals are
given by Sieverts and Bergner (1912).
ARSENIC 98
ARSENIC As.
Data for the fusion-points of mixtures of arsenic and iodine are given by
Jaeger and Doornbosch (1912).
MetaARSENIC ACID AsO2H.
DISTRIBUTION AT 25° BETWEEN:
(Auerbach, 1903.)
H2O and Amyl Alcohol. Sat. Aq. H3BO3 Solution and Amyl Alcohol.
Cms. AsO2H per 1000 cc. Gms. AsQ2H per 1000 cc.
Aq. Layer. Alcoholic Layer. Aq. Layer. Alcoholic Layer.
4.82 O.gO 9.28 1.75
9-63 i-75 18.74 3.47
18.44 3-5o
ARSENIC TriBROMIDE and TrilODIDE AsBr3 and AsI3.
100 gms. H2O dissolve about 6 gms. AsI2 at 25°. (U. S. P.)
100 gms. carbon disulfide dissolved about 5.2 gms. AsI3. (Squires.)
100 gms. methylene iodide, CH2I2, dissolve 17.4 gms. AsI3 at 12°, d of sat
Solution = 3.449. (Retgers, 1893.)
SOLUBILITY DATA DETERMINED BY THE FREEZING-POINT METHOD ARE GIVEN
FOR MIXTURES OF:
Arsenic tribromide and naphthalene. (Pushin and Kriger, 1914-)
" phosphorus triiodide. (Jaeger and Doornbosch, 1912.)
" triiodide and iodine. (Quercigh, 1912.)
ARSENIC TriCHLORIDE AsCl3.
When i.o gm. of arsenic as the trichloride is dissolved in 100 cc. of aq. HC1
and the solution shaken with 100 cc. of ether the following percentages of the
metal enter the ethereal layer; with 20% HC1, 68%; 15% HC1, 37%; 10%
HC1, 7%; 5% HC1, 0.7% and with i% HC1, 0.2% of the arsenic. (Mylius, 1911.)
ARSENIC TRIOXIDE As2O3.
SOLUBILITY OF THE:
Crystallized Modification. Amorphous Modification,
In Water. In Water.
. Gms.As203per
Sat. Solution. ioocc.H2O.
2 1 . 201 ord. temp. 3 . 7
15 1-657 b. pt. 11.86
25 ft 2 '°38 In Alcohol, Ether and CS2.
39'8 2.930 G.As203 per xoog. Solvent.
b-Pt- Alcohol 0.446
(Bfuner and St. Tolloczko — Z. anorg. Chem. 37, 456, Ether O . 454
'03; Chodounsky — Listy. Chem. 13, 114, '88.) £§ O.OOI
(Winkler — J. pr. Chem. [2] 31, 347, '85.)
SOLUBILITY OF ARSENIC TRIOXIDE IN AQUEOUS SOLUTIONS OF AMMONIA AT
30° (INTERPOLATED FROM ORIGINAL RESULTS).
(Schiememakers and deBaat, 1915.)
Gms. per 100 Gms. Sat Sol. Gms. per 100 Gms. Sat. Sol.
" Solid Phase. . - •• - " - . Solid Phase.
. .
NH3. AsjOg. NH3.
0 2.3 As2O3 4 7.6 NH4AsO4
1 8.3 " 5 6.2
2 14.9 " 7 4.6
2.8 20.5 As2O3+NH4AsO2 10 3.1
3 13 NH4As04 13 2.4
3-5 9-i 14-3 2.2
99
ARSENIC OXIDES
SOLUBILITY OF ARSENIC TRIOXIDE IN WATER AND IN ' AQUEOUS SOLUTION
OF HYDROCHLORIC ACID AT 15° (Interpolated from the original).
(Wood, 1908.)
Mols. HC1 per
Liter.
Gms. AsA per
100 cc. Solution.
0
0.46
1-495
2
1.2
4
1-3
Mols. HC1 per
Liter.
Cms. AsA per
100 cc. Solution.
6
3-8
7
7-5
8
12.5
9
17.7
SOLUBILITY OF ARSENIC TRIOXIDE IN AQUEOUS SALT SOLUTIONS.
(Schreinemakers and deBaat, 1917.)
In Aq. Ammonium Bromide at 30°.
Gms. per too Gms. Sat. Sol. ^ ^^
AsA
AsA-
NH4Br.
2.26
0
2.25
0-339
0.679
4-37
0.518
7.l8
0.386
I3-3I
0.303
2O.I4
0.237
31.69
0.154
41-34
0.190
45.66
0
44-8
As203.NH4Br
"+NH,Br
NI^Br
In Aq. Sodium Bromide at 30°.
Gms. per too Gms. Sat. Sol.
NH^Br.
2.19
5-57
AsA
2.09
10.89
"
1.88
20.79
«
1.63
30.39
"
1.50
35-75
"
1.20
39-24
(AsA)3NaBr
0-953
43.64
"
0.852
45-99
<(
0.719
50.25
" -f-NaBr.2:
0
±49-5
NaBr.2H2O
In Aq. Barium Bromide at 30°.
Cms. per too Gms. Sat. Sol.
In Aq. Barium Chloride at 30°.
AsA
2.09
2.03
BaBr2.
9.41
16.88
1.97
1.87
1.58
24.03
24.41
23.49
0-757
0.678
0.464
29.09
33-08
38.19
0.322
43-02
0.277
O
50.03
50.62
Cms. per 100 Cms. Sat. Sol.
' +BaBr2.2H2O
BaBr2.2H2O
AsA
BaCl2.
2.24
3-84
2. 2O
8.72
2.19
8.86
2-15
10.34
1.69
9-55
1. 12
13.62
0.905
16.93
0-737
20.06
0.608
23.87
0.506
26.54
0
27.6
Solid Phase.
AsA
(AsA)2.BaCl,
' +BaCl2.2H2O
BaCl2.2H2O,
In Aq. Calcium Bromide at 20°. In Aq. Calcium Chloride at I9.5°-2O°.
Gms. per 100 Gms. Sat. Sol.
Solid Phase.
As2 O3
CaBr2. '
1-58'
9.65
AsA
1.28
20.13
"
O.9I2
34-90
«
0.789
41
«
0.698
47.67
«
0-5I3
52.06
«
0.687
58.22
" +CaBr2.6H2O
0
58.20
CaBr2.6H2O
Gms. per 100 Gms. Sat. Sol.
AsA.
I.78
i-39
1. 01
0.865
0-757
0.697
0.675
O
CaClz.
O
12.66
23.09
27.68
31.85
36.01
41.92
42.7
Solid Phase.
AsA
100 gins. 95% formic acid dissolve 0.02 gm. AszO3 at 19.8°.
" +CaCl2.6H20
CaCl,.6H,O
(Aschan, 1913.)
ARSENIC OXIDES
100
SOLUBILITY OF ARSENIC TRIOXIDE IN AQUEOUS SALT SOLUTIONS. (Continued.)
In Aq. Lithium Bromide at 30°.
Gms. per 100 Gms. Sat. Sol. ^ ^^
AsA
In Aq. Lithium Chloride at 30°.
Cms. per too Cms. Sat. Sol.
AsA.
LiBr.
2.26
O
1.69
11.68
1.20
23-23
0-734
35-54
0-534
37
0.332
42.62
0.28l
43-87
0.198
46.75
0
59.62
+(As203)2.LiBr
(As2O3)2.LiBr
LiBr.H2O
AsA.
LiCl. '
LOOUU 1 IK1SC.
1.69
7-57
AsA
I-I5
15-30
«
0.77
22.67
«
0-54
29.04
it
0.43
35-37
"
0-39
41.13
"
0.385
43-oi
<«
0.41
45.12
" +LiCl.H2O
0
46.1
LiCl.H2O
In Aq. Potassium Bromide at 30°.
Gms. per 100 Gms. Sat. Sol.
In Aq. Potassium Iodide at 30**.
Solid
Gms. per 100 Gms. Sat. Sol.
Solid
'AsA-
2.25
0.8l8
0.460
0.327
0.290
0.275
0.207
0.166
0
KBr.
0.336
2.51
12.78
22.59
27.40
36-98
39 -°4
42.07
AsA+0
'AsA-
2.26
0.772
0.296
AsA
(AsA)2-KI
150
II9
"+KBr
KBr
0.081
0.115
0.134
D variesfrom (As2O3)2KBrto (As203)7(KBr)4. °
1 In Aq. Strontium Bromide at 30°.
Gms. per 100 Gms. Sat. Sol.
AsA-
.69
.74
.48
.25
.07
0.991
0
SrBr2.
1 1 . 69
22.09
31.98
41.91
46.87
48.91
49-H
AsA
As2O3.
2.14
1.92
1.67
1.46
I . 28
"+SrBr2.6H20 x . 23
SrBr2.6H2O O
ARSENIC PENTOXIDE As2O6.
SOLUBILITY IN WATER.
(Menzies and Potter, 1912.)
Solid Phase. t°.
Ice
KI.
O
I.I9
9-56
22.89
34-31
40.79
47.07
53-51
60.54
61.5
In Aq. Strontium Chloride at 30°.
Gms. per 100 Gms. Sat. Sol.
SrCl2.
6.27
13.67
21.29
27.46
34-03
36.16
37-5
"+KI
KI
Solid Phase.
AsA
+SrCl2.6H20
SrCl2.6H,0
- 5 10.6
— io 15.6
— 20 21.3 "
-30 25.1
— 40 27.8
-50 29.9
— 59 EutCC. 31.7 Ice+AsA4H20
— 50 32.6 AsA4H20
-40 33-5
-30 34-4
-20 35.4
100 gms. 95% HCOOH dissolve 7.6 gms.
— io
o
+ 10
20
29
40
60
80
100
120
140
36.2
37-3
38.3
39-7
41.4
41.6
42.2
42.9
43-4
43-7
44-5
Tol Solid Phase.
AsA4H20
"+3AsA.5H20
3As206.5H2O
19
(Aschan, 1913.)
ioi A&5FNIOCS r&lELFIDE
ARSENIOUS SULFIDE As^Ss.
looo cc. water dissolve 0.000517 gm. As2S3 at 1 8°. (Weigel, 1907.)
Data for the fusion-points of mixtures of arsenious sulfide and silver sulfide
are given by Jaeger and Van Klooster (1912).
ASPARAGINE C4H8N2O3.H2O.
SOLUBILITY /S-/-ASPARAGINE, C4H8N2O3.H2O, AND OF ^-/-ASPARAGINIC ACID,
C4H7NO4, IN WATER.
(Bresler — Z. physik. Chem. 47, 613, '04.)
/3-/- Asparagine. /3-/-Asparaginic Acid.
Gms.
t°. C4H8N203.H20 t°.
per 100 g.
Gms.
C4H8N203.H20 t
per loo g.
0
Gms.
C4H7NO4
per 100 g.
t
Gms.
'. C4H7NO4
per 100 g.
H2O.
H20.
H2O.
H2O.
0-7
0.9546
55-5
10.
650
0
.2
0-2674
51
• O
i
.2746
7-9
I . 4260
71.7
19.
838
9
•5
0.4042
63
•5
i
.8147
17-5
2.1400
87.0
36.
564
16
•4
0.5176
70
.0
2
•3500
28.0
3.1710
98.0
52-
475
31
•5
0-75*4
80
•5
3
.2106
41-4
5.6500
40
• o
0.9258
97
•4
5
•3746
) gms. H2O dissolve 2.4
gms.
asparagine at 2o°-25°.
(Dehn, 1917.)
100 gms. pyridine dissolve 0.03 gm. asparagine at 2o°-25°.
;ioo gms. 50% aq. pyridine dissolve 0.15 gm. asparagine at 2O°-25°.
loo gms. trichlorethylene dissolve o.oi 8 gm. asparagine at 1 5°. (Wester & Bruins, 1914-)
Data for the solubility of asparaginic acid in aqueous salt solutions are given
by Wiirgler (1914).
ASPIRIN (Acetyl salicylic acid) C6H4(OCH3CO)COOH.
loogms. water dissolve 0.25 gm. aspirin at room temperature. (Squire and Caines, 1905.)
loo cc. 90% alcohol dissolve 20 gm. aspirin at room temperature. "
ATROPINE
SOLUBILITY OF ATROPINE, Ci7H23NO3, AND OF ATROPINE SULFATE,
$ (CnH23NO3)2.SO2(OH)2, IN WATER AND OTHER SOLVENTS.
(U. S. P.; Muller, 1903.)
Grams Atropine per xoo Grams.
Solution. Solvent. (U. S. P.) Gf^|$Jlt
Water 25 1.782 (20°) 0.222 (0.13*) 263.1
Water 80 ... 1.15 454-5
Alcohol 25 ... 68.44 27
Alcohol 60 ... in. ii 52.6
Ether 25 2.21 (20°) 6.02 0.047
Chloroform 25 68.03 (20°) 64.10 0.161
Benzene 20 3.99
Carbon Tetrachloride 20 0.661
Ethyl Acetate 20 3 .88
Petroleum Ether 20 o . 83
Glycerol 15 ... 3 33
Aniline 20 ... 34§
Diethylamine 20 ... 67 §
Pyridine 20 ... 73§
Piperidine 20 ... H4§
50% Aq. Glycerol ) -r
+ 3%H3B03 j
Oil of Sesame 20 ... 0.25*
*Zalai, 1910. tAti7°,Schnidelmeiser,i9oi. JGori,i9i3. § Scholtz, 1912. IFBaroni and Borlinetto, 1911.
102
DISTRIBUTION OF ATROPINE BETWEEN WATER AND CHLOROFORM AT 25°.
(Seidell, 19100.)
Gms. Atropine Recovered per 15 cc.
per 15 cc. HssO+is cc.
CHCla.
Aqueous
Layer (a).
Chloroform
Layer (b).
b <
a
O.OO5
O.OOIO
0.0057
5-7
0.025
0.0021
0.0256
12.2
0.125
0.0049
o . i 246
25.4
0.625
0.0160
0.6267
39-i
ATROPINE METHYLBROMIDE
IOO gms. water dissolve IOO gms. of the salt at room temp. (Squires and Caines, 1905.)
100 cc. 90% alcohol dissolve 10 gms. of the salt at room temp. "
AZELAIC ACID C7H14(COOH)2.
SOLUBILITY IN WATER.
(Lamouroux, 1899.)
t°. = o 15 20 35 50 65
Gms. C7Hi4(CqOH)2
per 100 cc. solution = o.io 0.15 0.24 0.45 0.82 2 20
loo gms. 95% HCOOH dissolve 3.79 gms. azelaic acid at 19.4°. (Aschan, 1913.)
DISTRIBUTION OF AZELAIC ACID BETWEEN WATER AND ETHER AT 25°.
(Chandler, 1908.)
Gms. C7Hi4(COOH)j per 1000 cc.
Aq. Layer.
O.O6
Ether Layer*
0.47
1. 10
2.71
4.26
Gms. C7Hi4(COOH)2 per 1000 cc.
Aq. Layer. Ether Layer.
0.40 5.83
0.50 7.40
0.58 8.65
O.IO
0.20
0.30
AZOBENZENE C6H5.N2.C6H6.
SOLUBILITY OF AZOBENZENE IN SEVERAL BINARY MIXTURES.
(Timmermans, 1907.)
Solvent, Binary Mixture of: t°.
Gms. (CeHsN)? per
loo Gms. Sat.;Sol.
6.4
0.46
34.9% Butyric Acid + 65.1% H2O (= sat. sol.
10
IT *J
at 2.3°)
20
•I3
O /
30
i .92
40.6
2-95
80
.0
3.22
36% Triethylamine + 64% H2O (= sat. sol. at
II
2.57
19.1°)
14
1.66
17.4
°-54
69-3
0-43
36.5% Phenol + 63.5% H2O (= sat. sol. at
6-^°)
72.7
80
0.47
1.47
o o /
90
2-43
IOO
3-45
23-9
0.52
71.4% Phenol + 28.6% H2O (= sat. sol. at
20.6°)
25.2
40
0.87
4.45
60
10.35
72.6
I33-40
46% Succinic Nitrile-j- 54% H2O ( = sat. sol. at 54°) 56 . 9
0.54
103
AZOBENZENE
SOLUBILITY OF AZOBENZENE IN SEVERAL ALCOHOLS.
(Timofeiew, 1894.)
Solvent.
Methyl Alcohol 9 . 5
Ethyl Alcohol
9-5
Gms. (C6H3N)2
per loo Gms.
Solvent.
Gms. (C«HsN)2
t°. per 100 Gms.
Sat. Sol.
Sat. Sol.
3-8
Ethyl Alcohol
10.5 5.88
3-95
Propyl Alcohol
9-5 5-42
5-29
" "
10.5 6.02
SOLUBILITY OF AZOBENZENES IN WATER AND IN PYRIDINE.
(Dehn, 1917.)
Gms. Each Compound (Determined Separately) per
100 Gms. Solvent:
Solvent.
Water
Pyridine
Aq. 50% Pyridine
20-25
20-25
20-25
Azobenzene.
Diazoamino-
Dimethylamino-
benzene.
azobenzene.
0.03
O.O5
0.016
76.44
I36.7
27.90
16.78
67.7
4-Si
HydroxyAZOBENZENE C6H6.N: N.C6H4OH.
1000 cc. sat. solution in H2O contain 0.0225 gm. C6HsN: N.C6H4OH at 25°.
1000 cc. sat. solution in H2O sat. with C6H6 contain 0.0284 gm. C6H6N:N.
C6H4OH at 25°.
looo cc. sat. solution in C6H6 sat. with H2O contain 15.20 gms. C6H6N:N.
C6H4OH at 25°. (Fanner, 1901.)
Distribution results for hydroxyazobenzene between benzene and water gave:
cone, in C6H6 -*• cone, in H2O = 539 at 25°. (Farmer, 1901.)
AminoAZOBENZENE C6H6N: N.C6H4.NH2.
Distribution results for amino azobenzene between benzene and water gave:
COnc. in C6H6 -f- COnc. in H2O =3,173 at 25°. (Farmer and Warth, 1904.)
AZOANISOL, AZOBENZENE, AZOPHENETOL, etc.
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see footnote,
p. l), ARE GIVEN FOR THE FOLLOWING MIXTURES:
p Azoanisol Azobenzene
+ p Azoxyanisol (i)
-j- p Azoanisolphenetol (i)
+ Methylpropylazophenol (i)
" + p Azophenetol (i)
p Azoxyanisol
+ p Azoanisolphenetol (i)
+ p Azoxyphenetol (3), (4)
+ Benzene (2)
-j- Ethylene bromide (2)
+ Hydroquinone (5)
+ Benzophenone (5)
+ p Methoxycinnamic Acid (5)
-f Nitrobenzene (2)
p Azoanisolphenetol
to + Azophenetol (i)
+ p Dipropylazophenetol (i)
Azobenzene
+ Azoxybenzene (6)
+ p Azotoluene (7)
+ p Azonaphthalene (7)
-+- Benzalaniline (7)
p Azobenzoic Acid Ethyl Ester
+ p Azoxybenzoic Acid Ethyl
Ester (5)
(i) Bogojawlausky and Winogrodow, 1907; (2)
(3) Ratinjanz and Rotaiski, 1906; (4) Prins, 1909; (5)
(7) T
1907
Pascal and Normand, 1913; (8) Vanstone, 1913; (9) Beck, 1904; (10) Isaac (1910-11);
'; (12) Hasselblatt, 1913; (13) Garelli and Calzolari, 1899; (14) Bruni and Gorni, 1899.
+ Benzeneazonapthalene (9)
+ Benzil (8)
+ Benzoin (8)
+ Benzylaniline (7), (9), (10),
(n), (12)
+ Dibenzyl (7), (13), (14), (12)
+ Diphenyl (9)
-j- p Dimethoxystilbene (7)
+ Hydrobenzene (7)
+ Stilbene (7), (9)
+ Tolane (7)
Hydrazobenzene
+ Benzoin (8)
p Azophenetol
+ p Azoxyphenetol (i) '
-j- p Dipropylazophenetol (i)
p Azoxyphenetol
+ Cholesterylisobutyrate (A)
" + Cholesterylpropionate (4)
+ Cholesterylbenzoate (4)
" 4- P Methoxycinnamate (4)
p Azotoluene
+ Stilbene (7)
fawlauski, Winogrodow and Bogolubow, 1906;
Kock, 1904; (6) Hartley and Stewart, 1914;
(n) Jaeger,
AZOLITMINE
104
AZOLITMINE C7H7NO4.
100 gms. H2O dissolve 39.5 gms. azolitmine at 2O°-25°.
100 gms. pyridine dissolve 0.05 gm. azolitmine at 20-25°.
loo gms. aq. 50% pyridine dissolve 0.12 gm. azolitmine at 2O°-25°.
(Dehn, 1917.)
AZOPHENETOL (p) C^
SOLUBILITY IN 100 PER CENT ACETIC ACID.
(Dreyer and Rotarski — Chem. Centr. 76, II, 1016, '05.)
t°= 89.2 91 93 95«6 97-2 99-6
Mols. per liter. 0.153 0.176 0.185 0.209 0.232 0.252
A break in the curve at 94.7° corresponds to the transition temperature of the
a modification into the ft modification.
BARIUM ACETATE Ba(CH3COO)2. .
SOLUBILITY IN WATER.
(Walker and Fyffe, 1903; Krasnicki, 1887, gives incorrect* 'results.)
Gms. Ba(CH3COO)2
per 100 Gms.
Solid Phase.
Gms. Ba(CH3COO)2
per 100 Gms. Solid Phase.
Water.
Solution.
Water.
Solution
o-3
58
.8
37
.0
Ba(C2H302)2.3H20
40
•5
79
.0
44.1
Ba(C2H302)3
7-9
61
.6
38
.1
ft
41
•5
78
•7
44.0
u
17-5
69
.2
40
•9
1C
44
•5
77
•9
43-8
11
21 .6
72
.8
42
.1
(I
51
.8
76
•5
43-4
(I
24.1
78
.1
43
•9
11
63
.0
74
.6
42.7
1C
26.2
76
•4
43
•3
Ba(C2H302)2.H20
73
• o
73
•5
42.4
(C
30.6
75
.1
42
•9
«
84
.0
74
.0
42.5
cc
35-o
75
.8
43
.1
u
99
.2
74
.8
42.8
((
39-6
77
•9
43
.8
a
Transition temperatures 24.7° and 41°.
loo cc. 97% ethyl alcohol dissolve 0.0723 gm. barium acetate at room temp.
(Crowell, 1918.)
AQUEOUS SOLUTIONS OF ACETIC ACID
°
SOLUBILITY OF BARIUM ACETATE IN
AT 25
(Iwaki, 1914.)
5-18
Mols. per too Mols. Sat. Sol.
CHaCOOH.
Lo
0.41
1.40
1.46
3.30
10.23
20.60
(CH3COO)2Ba.3H2O
" +3.3.11
4.52
5.34
5.32
3.48
3.14
3.62
3(CH3COO)2Ba.3CH3COOH.iiH20,
3.3.11
Mols. per 100 Mols. Sat. Sol.
CHaCOQH.
28.72
36.54
42.08
46.51
51.98
65.77
85.27
7.85
8.87
8.62
8.40
7.36
;< +1.3
1.3
= (CH3COO)2Ba.3CH,COOH.
3.3.11
BARIUM ARSENATE Ba3(AsO4)2.
loo gms. H2O dissolve 0.055 gm. Ba3(AsO4)2; 100 gms. 5% NH4C1
dissolve 0.195 gm., and 100 gms. 10% NH4OH dissolve 0.003 Sm-
Ba3(AsO4)2
(Field — J. Ch, Soc. n 6, i8sp.)
BARIUM BENZOATE (C6H6COO)2Ba.6H2O.
100 gms. sat. aqueous solution contain' 4.3 gms. salt (anhydrous P)1 at 15°
and IO.I gms. at IOO°. (Tarugiand Checchi, 1901.)
105 BARIUM BORATE
BARIUM BORATES.
SOLUBILITY IN AQUEOUS BORIC ACID SOLUTIONS AT 30°.
(Sborgi, 1913.)
Cms. per ioo Gms.Sat. Sol. Cms. per 100 Cms. Sat. Sol.
• Ba2Q3. ' BaQ. Sohd Phase. . - t Sohd Phase.
3.6 0.04 H3B03+i.3.7 0.3 0.23 1.3.7
3.4 0.04 1.3.7 0.3 0.31 1.37+1.1.4
2.5 0.04 0.2 0.8 1.1.4
2.0 0.04 0.2 1.2
i.o 0.05 0.24 4.8 "
0.5 0.09 0.26 5.8 i.i4+Ba(OH)2
0.4 0.12 0.08 5.3 Ba(OH)2
1.3.7 = BaO.3B2O3.7H2O (Triborate); 1.1.4 = BaO.B2O3.4H2O (Metaborate).
The original results were plotted and above figures read from curve.
BARIUM BROMATE Ba(BrO3)2H2O.
SOLUBILITY IN WATER.
(Trautz>nd Anschiitz, 1906; Rammelsberg, 1841.)
Cms. Ba(BrO3)2 Cms. Ba(BrO3)2 Cms. Ba(BrO3)i
t. per ioo Gms, t°. per ioo Cms. t°. per ioo Cms.
Solution. Solution. Solution.
— 0.034 0.28 30 0-95 70 2.922
o 0.286 40 1.31 80 3-521
+ 10 0.439 5° J-72 90 4-26
20 0.652 60 2.271 98.7 5- .256
25 0.788 99.65 5.39
SOLUBILITY OF BARIUM BROMATE IN AQUEOUS SOLUTIONS OF SALTS AT 25°.
(Harkins, 1911.)
Cone, of Salt
in Gms. Equiv-
alents per Liter.
0
0.025
0.050
O. IOO
O.2OO
Gms.
Ba(BrOs)2 Dissolved per Liter in Aqueous Sol.
of
y
8
9
10
KI
93
62
91
25
JOa.
1.0038)
1.0059)
1.0080)
I. OI2O)
Ba(I
7-93
7.22
6.83
6.415
6 . 230
ro3)2.
1.0059)
1.0083)
1.0132)
1.0233)
7
5
3
i
KBrOs.
93
216 (1.0046)
415 (1.0062)
72 (1.0109)
7
8
Mg(NOs)2.
•93
.196(1.0114)
25°
Figures in parentheses show densities of the sat. sols, at — 5-*
4
BARIUM BROMIDE BaBr2.2H2O.
SOLUBILITY IN WATER.
(Kremers — Pogg, Ann. 99, 47, '56; Etard — Ann. chim. phys.frja, 540, '94.)
Gms. BaBr2 per TOO Grams. Gms. BaBr2 j>er ioo Grams.
t°. 'Water. Solution. t°. ' Water. Solution.
(Kremers.) (Kremers.) (Etard.) (Kremers.) (Kremers.) (Etard.)
—20 45-6 40 114 S3-2 S^S
o 98 49.5 47-5 50 II8 S4-i 52-5
10 101 50.2 48.5 60 123 55.1 53.5
20 104 51.0 49-5 70 128 56.1 54.5
25 106 51.4 50.0 80 135 57-4 55-5
30 109 52.1 50.6 ioo 149 60.0 57.8
140 ... 59.4
Sp. Gr. of saturated solution at 19.5° = 1.710.
BARIUM BROMIDE 106
Data for the system Barium Bromide + Barium Oxide + H2O at 25° are
given by Milikau (1916).
SOLUBILITY OF MIXTURES OF BARIUM BROMIDE AND BARIUM IODIDE IN WATER
AT DIFFERENT TEMPERATURES.
(Etard.)
Grams per ioo Gms. Solution. 0 Grams per too^Gms. Solution.
'
' BaBr2. BaI2. BaBr2.
— 16 4.8 58.4 170 ii. o 67.4
|-6o 5.5 66.0 210 14.9 67.7
135 9.2 67 . 2 Both salts present in solid phase.
SOLUBILITY OF BARIUM BROMIDE IN METHYL AND ETHYL ALCOHOLS.
(de Bruyn — Z. physik. Chem. 10, 783, .92 ; Richards — Z. anorg. Chem. 3, 455, '93 ; Rohland — Ibid.
15 412, '97.)
Parts BaBr2 per ioo Parts BaBr2.aH2O per ioo
o parts Aq. QjHfiOH of; parts of Aq. CH3OH of:
97%. »7%. i°o%. 93-5%. 50%.
15.0 .. 0.48 (BaBr2.2H20) .. 45.9 27.3 4.0
22.5 3 6 56.1
ioo gms. sat. solution in methyl alcohol at the crit. temp, contain 0.4 gm.
BaBr2. (Centnerszwer, 1910.)
Data for the lowering of the melting point of BaBr2 by BaF2 and by BaCl3
are given by Ruff and Plato (1903).
BARIUM PerBROMIDE BaBr4.
Data for the formation of barium perbromide in aqueous solutions at 25° are
given by Herz and Bulla (1911). See reference calcium perbromide, p. 189.
BARIUM BUTYRATE Ba(C4H7O2)22H2O.
SOLUBILITY IN WATER.
(Deszathy — Monatsh. Chem. 14, 249, '93.)
Gms. Ba(C4H7O2)2 per ioo Gms. Gms. Ba(C4H7O2)2 per ioo Gms.
**" Water. Solution". Water. Solution.
o 37-42 27.24 50 36.44 26.77
10 36.65 26.82 60 37.68 27.36
20 36.12 26.55 70 39-58 28.36
30 35.85 26.38 80 42.13 29.64
40 35-82 26.37
ioo gms. 97% ethyl alcohol dissolve 0.17 gm. barium butyrate at ord. temp.
(Crowell, 1918.)
BARIUM CAMPHORATE BaCioHi4O44H2O.
SOLUBILITY OF BARIUM CAMPHORATE IN AQUEOUS SOLUTIONS OF CAMPHORIC
ACID AT i6°-i7°.
(Jungflisch and Landrieu, 1914-)
Gms. per ioo Gms. Sat. Sol. Gms. per ioo Gms. Sat. Sol.
Camphoric Barium " SoUd Phase. Camphoric Barium Solid Phase.
Acid. Camphorate. Acid. Camphorate.
O.68 0.134 d Camphoric ac. + 1.3 0.48 22.71 1.3
0.84 0.150 " 0.45 32.19
0.693 0.20 1.3 0.50 37-22
0 . 38 2 . 59 " 0.51 40 . 99 1.3 + Ba Camphorate
O.44 II. IO " O 42.59 Ba Camphorate
1.3 = Barium tetracamphorate,
ID;
BARIUM CAPROATE
BARIUM CAPROATE AND BARIUM ISO CAPROATE.
SOLUBILITY IN WATER.
(Kulisch, 1893.)
Barium Caproate (Methyl 3 Pentan.)
Ba(CH3.CH2CH(CH3)CH2COO)2.
^ Gms.Ba(C6HuO2)2
40^ per 100 Gms. Solid Phase.
Water.
Solution.
0
11.71
10.
49 Ba(C6Hu02)2.3iH20
10
8.38
7-
73
20
6.89
6.
45
30
5-87
5-
55
40
5-79
5-
47
5°
6.63
6.
21
60
8-39
7-
74
70
11.09
9-
98
80
14.71
12 .
82
90
19.28
16.
16
(Konig, 1893.)
Barium Iso Caproate (Methyl 2 Pentan.)
Ba(CH3CH(CH3)CH2.CH2COO)2.
Gms. B3.(C(5rJiiO2/2
per loo Gms. gelid Phase.
Water.
Solution.
14-34
12
. 54 Ba(C6HuO2)2.4H2O
13-33
II
•77
12.67
II
.26
12.37
II
.01
12 .42
II
.05
12.83
II
.38
13 .63
II
•99
14.68
12
.80
16.24
13
•97
17-95
15
•23
BARIUM CARBONATE BaCOg.
SOLUBILITY IN WATER.
(Holleman, Kohlrausch and Rose, 1893.)
Electrolytic conductivity method used.
i liter H2O dissolves 0.016 gin. BaCO3 at 8.8°, 0.022 gm. at 18°, and 0.024 g™- at
24.2°.
SOLUBILITY OF BARIUM CARBONATE IN WATER CONTAINING CO2.
The average of several determinations at about 10°, by Bineau, Lassaigne,
Foucroy and Bergmann is i.io gms. BaCO3 per liter water. Wagner (Z. anal.
Ch. 6, 167, '67) gives 7.25 gms. BaCO3 per liter of water saturated with CO2 at
4-6 atmospheres pressure.
Eleven determinations by McCoy and Smith (1911), of the solubility of
barium carbonate at 25° in water in contact with pressures of CO2 varying from
0.2 to 30 atmospheres, showed that a maximum solubility is reached at 22 atmos-
pheres (see also calcium carbonate, p. 192), at which point the saturated solution
contains 0.727 mols. = 45.1 gms. H2CO3 per liter and 0.028 mols. = 7.3 gms.
Ca(HCO3)2 per liter. The equilibrium constant is k = 2.24 X IO"2 and the
solubility product Ba X CO3 = k* = 8.1 X lo"9.
SOLUBILITY OF BARIUM CARBONATE IN AQUEOUS SOLUTIONS OF AMMONIUM
CHLORIDE AT 30°.
(Kernot, d'Agostino and Pellegrino, 1908.)
Gms. per 1000 cc.
NH4C1.
O
8.0Q9
64-536
92-593
160.265
186.775
268.920
Solid
Phase.
BaCOs.
0.035 ° BaCOs
0.521
1-333
1.596
2
2.093
2.256
Data are also given for 25°. Some uncertainty exists as to the terms in which
the results are expressed. In some cases the column headings read "Gms. per
liter of H2O" and in others "Gms. per liter of solution." The saturation was
effected by adding just the necessary amount of one constituent to cause the
disappearance of the last particle of the other. The amounts so added were
determined by weighing the flasks. At high concentrations of the two salts, the
sudden increase in solubility appears to indicate a molecular combination.
Gms. per 1000 cc. HzO.
Solid
Phase.
BaCOs.
NH4C1.
2.245
335-70
BaCOa
2.706
358.66
"
2.630
418.33
NHiCl
2.I5I
414.71
1.558
4I3-77
"
0.730
4IO.I6
u
0
397-58
"
BARIUM CARBONATE
108
SOLUBILITY OF BARIUM . CARBONATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AND OF SODIUM CHLORIDE.
(Cantoni and Goguelia, 1905.)
In KClatB.pt. of Sol. In NaCl at B.pt. of Sol. In 10% KC1 Sol. In io%NaC!Sol.
Cms. KC1
per 100
Cms. Sol.
0.15
1. 00
3
IO
30
Cms. BaCOs
per 1000 cc.
Sat. Sol.
Gms. NaCl Gms. BaCOs
Gms. BaCOa
Gms. BaCOs
per 100
Gms. Sol.
per 1000 cc.
Sat. Sol.
t.
per 1000 cc.
Sat. Sol.
t°.
per 1000 cc.
Sat. Sol.
0.15
0.0587
10
0.2175
10
0.1085
I
0.0787
2O
o . 2408
20
O.II26
3
0.1056
40
0.2972
40
0.1231
10
0-1575
60
0-3491
40
0.1303
30
0.2784
80
o . 4049
40
0.1418
o . 0847
o. 1781
0.2667
0.4274
0-5550
Barium carbonate boiled with aqueous NH4C1 is slowly but completely decom-
posed. The time required varies inversely as the concentration of the NH^Cl
solution.
Data are also given for solubility in 10% aqueous KC1 and NaCl at the boiling
point, the time factor being varied from I to 198 hours.
Data for lowering of the melting point of BaCO3 by Na2CO3 are given by Sackur
(1911-12).
BARIUM CHLORATE Ba(ClO3)2.H2O.
SOLUBILITY IN WATER.
(Carlson, 1910; Trautz and Anschiitz, 1906.)
fo Sp. Gr. of Cms. Ba(ClO»)j per 100 Sp. Gr. of
*• Sat. Sol. Gms. Sat. Sol. t. Sat. Sol.
Gms. Ba(C103)2 per too
Gms. Sat. Sol.
O
IO
20
25
30
1 . 195 2O
24
1.274 28
30
32
3*
3
2
16.90!'
21.23
25.26
27-53
29-43
* C.
40
60
80
100
105 . 6 b. pt.
t (rand 4.)
•355
•433
-508
-580
.660
35
42
48
53
54
8*
6
i
6
33
40
45
Si
52
i6f
05
90
2
62
The determinations of Trautz and Anschiitz appear to have been made with
very great care. The original paper of Carlson was not available and it has
been impossible to explain the discrepancy between the two sets of results.
BARIUM PerCHLORATE Ba(C104)2.3H2O.
SOLUBILITY IN WATER.
(Carlson, 1910.)
O
20
40
60
Sp. Gr.
Sat. Sol.
1.782
1.912
2.009
2.070
Gms. Ba(C104)2
per 100 Gms.
Sat. Sol.
67-3
74-3
78.2
81
80
100
1 20
140
Sp. Gr.
Sat. Sol.
2.114
2.155
2.195
2.230
Gms. Ba(C104)2
per too Gms.
Sat. Sol.
83-2
84.9
86.6
88.3
BARIUM CHLORIDE BaCl2.2H2O.
SOLUBILITY IN WATER.
(Mulder, Engel, 1888; Etard, 1894.)
,„ Gms. BaCla per 100 Gms.
O
10
20
25
30
40
50
Water.
31-6
33-3
35-7
3£
38.2
40.7
43-6
Solution.
24
25
26.3
27
27-7
28.9
3°-4
60
70
80
IOO
130
1 60
215
Gms. Bad? per TOO Gms.
Sp. Gr. of solution saturated at o° = 1.25; at 20°
Water.
Solution.
46.4
31-3
49-4
33-i
52.4
34-4
58.8
37
59-5
"37-3
63-6
38.9
75-9
43-1
1.27.
109
BARIUM CHLORIDE
SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND AMMONIUM CHLORIDE
IN WATER.
At 30°. (Schreinemakers, 1908.)
Cms, per'ioo Cms. Sat. Sol
' BaCb. NH4C1.
22.16 5.71
18.36 10.06
15.42 13.84
10.89 20.01
8.33 24.69
7-97 25.92
3-S6 27.47
Solid Phase.
BaCl2.2HjO
BaCh.2H20+NH4Cl
NH4C1
At Varying Temps. (Schreinemakers, igiob.)
Cms. per too Cms. Sat. Sol.
Solid Phase.
BaCU.2HjO+NH4Cl
t
16.2
o
30
40
So
BaCl2.
8.07
8.22
8.19
8.40
8-55
NH<C1.
16.10
19.26
24.89
26.93
29-53
SOLUBILITY OF BARIUM CHLORIDE IN AQUEOUS SOLUTIONS OF BARIUM
HYDROXIDE AND VICE VERSA AT 30°.
(Schreinemakers, 1909-1910, igiob.)
Gms. per roo'Gms. Sat. Sol.
BaClz.
BaO.
27.6
O
BaCI2.2H20
27.42
1.78
"
,57.36
1.77
" +BaCl(OH).2H2O
'24.98
2-33
BaCl(OH).2H2O
21.46
3-27
«
19.18
4.67
it
BaCl2.
BaO.
ia rnase
18.67
4.61
BaCl(OH).2
HjO+B
18.04
4.62
BaO.gHjO
17.08
4.60
"
12. 8l
4.58
M
10.77
4-45
«
O
4-99
U
SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND BARIUM NITRATE
IN WATER:
At 30°. (Coppadoro, 1912, 1913.)
Gms. per 100 Gms. Sat. Sol.
BaCl2.
6.06
13-75
16.14
22.70
26. II
26.64
26.91
27.38
Ba(NO3)2.
9-55
8.20
7.92
7-94
7.88
5-37
4-13
1.58
Solid
Ba(NO»)i
Ba(NO3)j+BaCl2.2H2O
BaCl2.2HzO
At Varying Temps. (Etard, 1894.)
Gms. per 100 Gms. Sat. S
S' Solid Phase.
BaCl2.
Ba(NOs)2.
O
22.5
4-3
BaCU.2H2O+Ba(NO»)»
20
24-5
6
"
40
26.5
7-5
"
60
28.5
9-5
«<
IOO
31
14
"
140
32
20
"
180
33
26
•
210
32
32
"
SOLUBILITY OF BARIUM CHLORIDE IN AQUEOUS SOLUTIONS OF COPPER
CHLORIDE AT 30° AND VICE VERSA.
(Schreinemakers and de Baat, 1908-09.)
Gms. per 100 Gms. Sat. Sol.
BaCU.
O
1-25
3.08
2.72
2.84
3.98
CuCl2.
43-95
42.45
42.07
42.36
41.18
37-42
Solid Phase.
CuCli.2H2O
(unstable)
CuCk. 2H2O +BaCl2. 2H«0
BaCli.2HiO
jiiis. per it>o
\jins. oat. oui-
. Solid Phase.
BaCk.
CuCl2.
5-49
30.76
BaCk^HsO
10.13
21.76
•
17.08
11.49
"
22.78
•5-13
«
27.6
O
it
Solubility data have been determined for the following systems:
BaCl2.2H2O 4- CuCl2.2H2O + NH4C1 + H2O at 30°. (Schreinemakers, 1909.)
+ " 4- KC1 + H2O at 40° and 60°. ( " and de Baat, 1914.)
4- " + NaCl + H2O at 30°. ( " and de Baat, 1908^9.)
+ BaO + Na2O + H2O at 30°. (Schreinemakers, igiob.)
4- Ba(NO3)2 4- NaNO3 + NaCl + H2O at 30°. (Coppadoro, 1913.)
4- HCl 4- NaCl 4- H2O at 30°. CSchreinemakers, 1909-10. igiob.)
BARIUM CHLORIDE
no
SOLUBILITY OF BARIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
CHLORIC ACID:
Ato°.
(Engel, 1888.)
At 30°.
(Masson, 1911, 1912-13; Schreinemakers, 1909-10.)
>p. Gr
Gms. per 100
jms. Sat. Sol. «
at. Sol.
' HC1.
BaCli. ' S
.250
'o
24.07 I
.242
0.32
23-3I
.228
0.83
22.11
.2IO
I-5I
2O.I4
•143
4.58
12.76
.118
6.13
9-37
.099
7-55
6-33
.079
10.81
2.64
.088
16.92
0.28
Sp. Gr.
Sat. Sol.
Gms. per 100 Gms. Sat. Sol.
1.3056
.2651
.2147
-1789
.1419
.io68
.o88o
.0895
1024
.!6o9
The results of Schreinemakers show that at 37.34% HC1 the barium chloride
dihydrate is converted into monohydrate.
Less than i part of BaCl2 is soluble in 20,000 parts of concentrated HC1 and in
120,000 parts of cone. HCl containing | volume of ether. (Mar, 1892.)
SOLUBILITY OF BARIUM CHLORIDE IN AQUEOUS SOLUTIONS OF MERCURIC
CHLORIDE:
HC1.
BaCb.
0
97.84
1.36
24.02
3-32
19.20
5-oi
IS-2
7-13
II. I
10
5-8
13-43
2.4
16.92
0.38
20.62
o
32.18
o
At O°. (Schreinemakers, 1910.)
Gms. per 100 Gms. Sat. Sol.
At 30°. (Schreinemakers, 1910.)
' HgCl*.
BaCh.
0
23.70
14.25
24
36.20
24.89
46.08
24.05
46.59
23.28
47-78
21.05
48.46
20.67
44-33
18.50
29
"•59
16.36
6. ii
3-95
o
Solid Phase.
BaClt.2HjO
BaClt.3HgClj.6HjO
" +HgCl«
HgClj
SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND MERCURIC
CHLORIDE IN WATER.
(Foote and Bristol — Am. Ch. J. 32, 248, '04.)
HgCh.
BaCk.
oouu jriiase.
O
27.77
BaClj.2HjO
2.90
27.56
"
12.98
26.99
«
34-57
26.69
«
46.50
25.22
"
55-22
23.17
" +HgCl«
48.97
17.87
HgClj
41-30
14.26
"
27.62
8.4I
«i
14.19
2.65
«
7-67
O
"
Gms. per 100 Gms.
t°. Solution.
Solid
Phase.
BaCl2.
Hgci2:
10.4
23-58
50.54
( BaCl,2H,O+
I HgCl,.
10.4
10-4
10.4
23-44
22.58
22.48
50-74
51-23
51.41
( Double Salt
Gms. per 100 Gms.
t°. Solution.
Solid
Phase.
BaCl2.
HgCl2.
10.4
22.10
51.66]
[ Double Salt
IO-4
25
21.64
23.02
51-74.
54.83
( BaCl,.2H,O+HgCl8.
SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND SODIUM CHLORIDE
IN WATER:
At 30°.
(Schreinemakers and de Baat, 1908-09.)
Gms. per 100 Gms,
Sat. Sol.
BaCh. NaCl. '
O 26.47
2.28 25.28
3.80 23.77
5.76 20.25
8.19 17.89
Solid Phase.
Gms. per 100 Gms.
Sat. Sol.
NaCl
' +BaCU.2HiO
BaCb.2HiO
BaCk.
12.25
15-83
20.93
24.24
27.60
NaCl.
13-39
10.06
5-39
2.76
o
Solid Phase.
BaClZ.2H20
At Varying Temps.
(Precht and Wittgen, 1881 ;
Rudorff, 1885.)
Gms. per 100 Gms'
*o Sat. Sol.
20
40
60
80
100
BaCk.
2-9
4.5
6.8
9-4
ii. 8
NaCl.
25
23
23-4
22.8
22.2
in BARIUM CHLORIDE
SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND POTASSIUM CHLORIDE
IN WATER. (Foote, 1904.)
100 gms. saturated solution contain 13.83 gms. BaCl2 + 18.97 gms. KC1 at 25°.
Fusion-point curves (solubility, see footnote, p. i) are given for the following
mixtures:
BaCl2
+ BaCOs (Sackur, 1911-12.)
+ BaCrO4
-j- BaO (Sackur, 1911-12, Arndt, 1907.)
-j- BaSO4 (Sackur, 1911-12, Ruff and Plato, 1903.)
-j- BaF2 (Botta, 1911; Ruff and Plato, 1903; Plato, 1907.)
+ BaI2 (Ruff and Plato, 1903.)
+ CdCl2 (Sandonini, 1911, 1914; Ruff and Plato, 1903.)
-j- CaCl2 (Sandonini, 1911, 1914; Ruff and Plato, 1903; Schaefer, 1914.)
-j- CuCl2 (Sandonini, 1914-)
-j- PbCl2 (Sandonini, 1911, 1914; Ruff and Plato, 1903.)
-f- LiCl (Sandonini, 1913, 1914-)
-|~ MgCl2 (Sandonini, 1912, 1914.)
-j- MnCl2 (Sandonini, 1912, 1914; Ruff and Plato, 1903.)
-f- KC1 (Sandonini, 1911; Ruff and Plato, 1903; Vortisch, 1914.)
+ NaCl (Sackur, 1911-12; Ruff andPlato, 1903; LeChatelier, 1894; Vortisch, 1914.)
+ NaCl-f-KCl (Vortisch, 1914 («); Gemsky.)
4* SrCl2 (Sandonini, 1911, 1914; Ruff and Plato, 1903; Vortisch, 1914.)
-j- ZnCl2 (Sandonini, 1912 a, 1914.)
-f T1C1 (Korreng, 1914.)
SOLUBILITY OF
At 15°.
(Schiff, 1861;
'Rohland, 1897.)
Wt £« Gms.BaCk
r Tilr\u Per 100 Gms.
C2H{OH- Solvent.
10 31 -i
20 21.9
3° H-7
4O IO.2
60 3-5
80 0.5
97 0.014
BARIUM
Gms. per
Sat.
CHLORIDE IN AQUEOUS ETHYL ALCOHOL SOLUTIONS.
At 30°. At 60°.
(Schreinemakers and Messink, 1910.)
loo Gms. Gms. per 100 Gms.
Sol. Solid Phase. Sat. Sol. Solid Phase.
C^OH.
o
32.67
50.16
60.72
92-53
94-73
97-14
98.17
99.41
BaCk.
27 95
10.63
5-68
2.23
0.05
0.06
0.08
BaCk.2H20
" +BaCk.H2O
BaCk-HbO
" -f-BaCk
BaCla
C^OH.
0
16.68
34.10
66.02
88.55
90.25
93-95
BaCk.'
31-57
20.16
13.21
2.82
0.25
0.09
BaCk.2HzO
" +BaCk.H20
BaCk-HzO
100 gms. methyl alcohol dissolve 2.18 gms. BaCl2 at 15.5° and 7.3 gms. BaCl2.
2 H2O at 6°. (de Bruyn, 1892.)
loo gms. glycerol dissolve 9.73 gms. BaCl2 at i5°-i6°. (Ossendowski, 1907.)
loo cc. anhydrous hydrazine dissolve 31 gms. BaCl2 at room temp.
(Welsh and Broderson, 1915.)
100 gms. 95% formic acid dissolve 7.3 gms. BaCl2 at 19°. (Aschan, 1913.)
One liter sat. sol. in nitrobenzene contains 0.167 gm« BaCl2 at 20°, 0.33 gm. at
50° and 0.40 gm. at 100°. (Lloyd, 1918.)
Data for the system BaCl2 + Triethylamine + H2O are given by Timmermans
(1907).
SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND GLYCINE. IN WATER
AT 2O°. (Pfeiffer and Modelski, 1912.)
Gms. per 100 cc. Sat. Sol.
Nft2CH2COOH.
5-5
26
BaCk
37
16
Solid Phase.
BaCU. 2H2O+BaCk. 2NH2CH2COOH.HjO
NH4CHjCOOH+BaClj.2NH2CHjCOOH.HaO
BARIUM CHROMATE
112
BARIUM CHROMATE BaCrO4.
SOLUBILITY OF BARIUM CHROMATE IN WATER.
One liter of sat. solution contains 0.002 gm. of the salt at o°; 0.0028 gm. at
10°; 0.0037 gm. at 20° and 0.0046 gm. at 30°. (Kohkausch, 1908.)
Results higher than the above are given by Schweitzer, 1890, as follows:
One liter of aqueous solution saturated at room temp, contains o.oi gm. BaCrO4;
if ignited barium chromate is used, only 0.0062 gm. dissolves.
One liter sat. sol. contains 0.043 Sm- °f the salt at boiling point. (Mescherzski, 1882.)
Fresenius (1890) gives the following: i liter of sat. sol. at room temp, con-
tains 0.02 gm. of the salt, the solvent being 1.5% sol. of CH3CO2NH4 and 0.022
gms. when the solvent is 0.5% sol. of NH4NO3.
One liter of 45% aq. ethyl alcohol solution dissolves 0.000022 gm. at room temp.
BARIUM CINNAMATES. (Guenm, I9i2.)
SOLUBILITY OF BARIUM CINNAMATES IN WATER, METHYL" ALCOHOL AND ACETONE.
Gms. Anhy-
Authority.
o. 726 (Tarugi and Checchi, 1901.)
(Liebermann,i903.)
(Michael and Garner, 1903.)
(Michael, 1901.)
(Michael and Garner, 1503.)
(Michael, 1901.)
Compound.
Formula. t°.
Solvent.
arous o
Der ioo G
Sat. Sc
Barium Cinnamate
Ba(C9H702)2.2H20 15
HjO
0.72*
u
"
" IOO
"
2.27
"
Allocinnamate
Ba(C9H7O2)2.H2O 19
CHsOH
15.8
"
u
12
"
I5-4
"
"
Ba(C»H7O2)j3HjO 20
"
2.56
II
"
" 2O
(CH3)zCO
0.80
"
"
" 2O
HzO
6
"
Hydrocinnamate
Ba(C9H70J)2.2HiO 27
"
2.9
"
«
25
CHsOH
O.I
"
"
16
"
9-7
"
Isocinnamate
20
*
70
"
"
20
(CHs)2CO
20
u
"
20
HjO
17
BARIUM
CITRATE Ba3(C6H6O7)2.7H2O.
SOLUBILITY IN WATER AND IN ALCOHOL.
ioo grams water dissolve 0.0406 gram Ba3(C6H6O7)2.7H2O at 18°,
and 0.0572 gm. at 25°.
ioo grams 95% alcohol dissolve 0.0044 gram Ba3(C6H6O7)2.7H2O at
18°, and 0.0058 gm. at 25°.
(Partheil and Hiibner — Archiv. Pharm. 241, 413, '03.)
BARIUM CYANIDE Ba(CN)2.
SOLUBILITY IN WATER AND IN ALCOHOL AT 14°.
(Joannis — Ann. chim. phys. [5] 26, 489, '82.)
ioo parts water dissolve 80 parts Ba(CN)2.
ioo parts 70% alcohol dissolve 18 parts Ba(CN)2.
BARIUM FERROOYANIDE AND BARIUM POTASSIUM FERRO-
CYANIDE.
(Wyrouboff — Ann. chim. phys. [4] 16, 292, '69.)
ioo parts water dissolve o.i part Ba3Fe(CN)6.6H2O at 15°, and i.o
part at 75°.
ioo parts water dissolve 0.33 part BaK2Fe(CN)0.5H2O at ord. temp.
BARIUM FLUORIDE BaF2.
SOLUBILITY IN WATER.
» (Kohkausch, 1908.)
One liter sat. sol. contains 1.586 gms. of the salt at 10°; 1.597 gms. at 15°;
1.607 g1115- at 2°°j 1-614 gms« at 25° and 1.620 gms. at 30°.
Freezing-point curves are given for mixtures of BaFz+KF by Puschin and
Baskow (1913), and for BaF2-J-BaIj by Ruff and Plato (1903).
BARIUM FORMATE
BARIUM FORMATE Ba(HCOO)2.
SOLUBILITY IN WATER. (Stanley, 1904. See also Krasnicki, 1887.)
Gms. Ba(HCOO)j to
2r too Gms. Sat. Sol.
per
Gms. Ba(HCOO)«
per zoo Gms. Sat. SoL
23.24
23.22
O
10
20 23.0<
25 23.9
30 24.2
BARIUM HYDROXIDE Ba(OH)2.8H2O.
SOLUBILITY IN WATER. SOLID PHASE Ba(OH)2.8H2O.
40
So
60
80
100
25
25-9
26.9
29-3
32.8
(Rosenthiel and Riihlmanu '— Jahresber. Chem. 314, '70.)
Gms. Ba(OH)z per 100 Gms.
Gms. Ba(OH)2 per 100 Gms.
Water.
Solution
0
1.67
I . 6C
5
I .95
I • 02
10
2.48
, 2 .42
15
3-23
3-13
20
3-89
3-74
25
4-68
4-47
Water.
Solution.
30
5-59
5 -29
40
8.22
7.60
50
13.12
ii .61
00
20-94
17.32
75
63-51
38.85
80
101 .40
50-35
Data are given by Sill (1916), for the influence of pressures up to 490 kgs. per
sq. cm. on the solubility of Ba(OH)2.8H2O in H2O at 25°.
Sat. Sol.
.0512
.0651
.0790
•0975
.1220
SOLUBILITY OF BARIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF BARIUM
NITRATE AT 25° AND VICE VERSA. (Parsons and Carson, 1910.)
Sp. Gr. Gms. per 100 Gms. H2O. Solid Sp. Gr.
Ba(OH)2. Ba(NO3)2. Phase- Sat- So1-
4.29 O Ba(OH)j.8H2O I.I37I
4.35 1.88 " 1.1448
4.48 3.47 " I.I2IO
4.40 5-66 " I.IOO2
4-72 7-55 " 1-0797
Ba(OH)2.Ba(NO3)2.
4.93 10.21
5.02 11.48
Phase.
Ba(OH)2.8H2O
" +Ba(N03)a
3-22 11.04
1.55 10.66
Ba(N03)8
o 10.30
«
SOLUBILITY OF BARIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF ALKALI
CHLORIDES AT 25°. (Herz, 1910.)
In Lithium
Chloride.
Gms. per 100 cc. Sat. Sol.
In Potassium
Chloride.
Gms. per 100 cc. Sat. Sol.
In Rubidium
Chloride.
Gms. per loqcc. Sat. Sol.
In Sodium
Chloride.
Gms. per loocc. Sat. Sol.
Lid.
9-75
6. 02
3-i8
o
Ba(OH)2. "
n-45
8.03
6-39
4.76
KC1.
25-95
I3-05
8.60
0
Ba(OH)2.
5-93
5-66
5-53
4.76
' RbCl.
15.11
0
Ba(OH)2.
5-55
4.76
NaCl.
16.51
8-37
4-27
0
Ba(OH)i".
6.91
5-99
5-40
4.76
SOLUBILITY OF BARIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF SODIUM
> HYDROXIDE AT 30°. (Schreinemakers, 1909-10.)
Gms. per 100 Gms. Sat. Sol.
BaO.
NacO.
4-99
O
1.29
4.78
0.89
6-43
0-57
9.63
0-53
11.62
0.47
17.87
1. 06
23.28
1.87
24.63
Solid Phase.
Gms. per 100 Gms. Sat. Sol.
Ba0.9H20+Ba0.4HjO
BaO.
NazO. '
ouuu riiitsc.
1.84
26.14
BaO.4H2O
i-75
27.72
"
1.58
28.43
"
i-34
29.24
" +Ba0.2H20
0.82
32.12
BaO.2H2O
0-59
34.72
"
o-57
41.09
" +NaOH.H«O
0
+42
NaOH.HiO
BARIUM HYDROXIDE 114
SOLUBILITY OF BARIUM HYDROXIDE IN AQUEOUS ACETONE AT 25°.
(Herz and Knoch — Z. anorg. Chem. 41, 321, '04.)
r t v i of Ba(OH)2 per 100 cc. Sat. Gms. Ba(OH)2
Sp. Gr. of Vol.% Solution. per
Solutions. Acetone. , — — • . xoo Gms.
Millimols. Grams. Solution.
1.0479 o 55.08 4.722 4.506
i. 0168 10 31-84 2.730 2.686
0.9927 20 17.79 i-S2S I-536
0.9763 30 9.10 0.779 0.798
0.9561 40 4.75 0.407 0.426
0.9398 50 1.54 0.132 0.141
0.9179 60 0.48 0.041 0.045
0.8956 70 0.08 0.007 0.018
Data for the systems Ba(OH)2 + Phenol + H2O at 25° and Ba(OH)2 +
Resorcinol + H2O at 30° are given by van Meurs (1916).
BARIUM IODATE Ba(IO3)2.H2O.
SOLUBILITY IN WATER.
(Trautz and Anschutz, 1906.)
to Gms. Ba(IO3)2 per „ Gms. Ba(IO3) per ±0 Gms. Ba(I03)2 per
100 Gms. Solution. 100 Gms. Solution. 100 Gms. Solution,
- 0.046 O.OOS 30 0.031 70 0-093
+ io 0.014 40 0.041 80 0.115
2O O-O22 5O 0.056 9O O.I4I
25 0-028 60 0.074 100 o>197
One liter sat. aqueous solution contains 0.3845 gm. Ba(IO3)2 at 25°.
(Harkins and Winninghoff, 1911.)
At room temperature Hill and Zink (1909), found 0.284 gm. Ba(IOs)2 per liter
sat. aqueous solution.
SOLUBILITY OF BARIUM IODATE IN AQUEOUS SALT SOLUTIONS AT 25°.
(Harkins and Winninghoff, 1911.)
Added Mols. Salt
Salt. per Liter.
Ba(NOs)2 o . ooi
0.002
" 0.005
" O.O2O
" o . 050
loo cc. cone, ammonia (Sp. Gr. 0.90) dissolve 0.0199 gm. Ba(IOs)2 at room
temp. (Hill and Zink, 1909.)
100 cc. 95% ethyl alcohol dissolve o.oon gm. Ba(IO3)2 at room temp.
(Hill and Zink, 1909.)
BARIUM IODIDE BaI2.
SOLUBILITY IN WATER.
(Kremers — Pogg. Ann. 103, 66, 1858; Etard — Ann. chim. phys. [7] 2, 544, '94.)
Gms-BaI2RerzooGms. ^ Gms ,.BaI2 per xooGms.
Water. Solution. Water. Solution.
-20 143-9 59-0 BaI2.6H.5O 40 231.9 69.8 BaI2.2 H2O
o 170.2 63.0 60 247.3 71-2
+ 10 185.7 65.0 80 261.0 72.3
20 203.1 67.0 100 271.7 73.1
25 212.5 68.0 " 120 281.7 73.8 "
30 219.6 68.7 160 294.8 74.6 "
Sp. Gr. of sat. solution at I9°.5 = 2.24.
100 gms. 95% HCOOH dissolve 75 gms. BaI2 at 20.2°. (Aschan, 1913.)
100 gms. 97% ethyl alcohol dissolve 1.07 gms. BaI2.2H2O at 15°. (Rohland, 1897.)
Data for the system BaI2+BaO+H2O at 25° are given by Milikau (1916).
Gms.
Ba(IO3)2
per Liter.
Added
' Salt.
Mols. Salt
per Liter.
Gms.
Ba(I03)2
per Liter.
Added
Salt.
Mols. Salt
per Liter.
Gms.'
Ba(I03)j
per Liter. ,
0-331
Ba(NO3)2
O.IOO
o. 148
KNO3
O.2OO
0.777
0.294
"
0.200
0.136
KIO3
O.OOOIO6
0.368
0.237
KNO3
O.OO2
0.396
"
0.000530
0.303
o. 164
"
O.OIO
0-445
"
o. 001061
0.229
0.149
"
0.050
0.643
115 BARIUM PerlODIDE
BARIUM PerlODIDE BaI4.
Data for the formation of barium periodide in aqueous solutions at 25° are
given by Herz and Bulla (1911). (See reference calcium perbromide, p. 186.)
BARIUM IODOMERCURATE.
A saturated solution of BaI2 and HgI2 in water at 23.5° was found by Duboin
(1906) to have the composition BaI2.i.33HgI2.7.76H2O, d = 2.76.
BARIUM MALATE BaC4H4Os.
SOLUBILITY IN WATER.
(Cantoni and Basadonna — Bull. soc. chim. [3] 35, 731, '06.)
to Gms.BaC4H4O5 to Gms. BaC4H4O5 to Cms. BaC4H4O8
per 100 cc. Sol. per 100 cc. Sol. per 100 cc. Sol.
20 0.883 35 0.895 60 i. on
25 0.90! 40 0.896 70 I.04I
30 0.903 50 0.942 80 1.044
SOLUBILITY IN WATER AND IN ALCOHOL.
(Rartheil and Hiibner — Archiv. Pharm. 241, 413,. '03.)
ioo grams water dissolve 1.24 gms. BaC4H4O6 at 18°, and 1.3631
gms. at 25°.
too grams 95% alcohol dissolve 0.0038 gms. BaC4H4O6 at 18°, and
0.0039 gm. at 25°.
BARIUM MALONATE BaC3H2O4.2H2O.
SOLUBILITY IN WATER.
(Miczynski — Monatsh. Chem. 7, 263, '86.)
Gms . BaC3H2O4 per ioo Gms. A „ Gms. BaC3H2O4 per too Gms.
t .
O
10
2O
30
40
Results slightly higher than the above, from o°-5O° are given by Cantoni and
Diotalevi (1905).
BARIUM MOLYBDATE BaMoO4.
ioo parts water dissolve 0.0058 part BaMoC>4 at 23°. (Smith and Bradbury, 1891.)
Water.
Solution.
» *
Water.
Solution.
0-143
0.143
50
0.287
0.285
0.179
0.179
60
0.304
0.303
0-212
0-2II
70
0.317
0.316
0.241
0.240
80
0.326
0-325
0.266
0.265
IARIUM NITRATE Ba(NO3)2.
SOLUBILITY
IN WATER.
(Mulder; Gay Lussac; Etard — Ann. chim. phys.ty] 2, 528, 94; Euler — Z. physik. Chem. 49, 3i5.'o4->
Gms. Ba(NO3)2
t°. per ioo Gms.
80
IOO
120
Gms. Ba(NO3)2
per ioo Gms.
Water. Solution.
o 5.0 4.8
10 7.0 6.5
20 9-2 8.4
Water. Solution.
27.0 21-3
• 34-2 25.5
42.0 29.6
25 10.4 9-4
30 ii. 6 10.6
40 14.2 12.4
50 17.1 14.6
60 20.3 16.9
140
160
180
200
215
5o-o 33-3
58.0 36.7
67.0 40.1
76.0 43.2
84.5 45.8
Results from o°-35° differing from the above are given by Vogel (1903).
ioo gms. sat. aqueous solution contains 4.74 gms. Ba(NO3)2ato°. (Coppadoro.ign.)
BARIUM NITRATE
116
SOLUBILITY OF MIXTURES OF BARIUM NITRATE AND LEAD NITRATE IN WATER
AT 25°. (Fock, 1897; Euler, 1904.)
In Solution.
>p. W. 01
Solution.
Cms.
per Liter.
Mg. Mols.
per Liter.
Mol. %
Mol.%
T> _/"VTr\ A
Ba(N03)2.
Pb(N03)2."
Ba(NO3)2.
Pb(N03)2"
Ba(NO3)2.
*>a^iN Usja
1.079
102.2
O
391.0
0
100
100
I .088
54-9
17.63
2IO.I
53-3
79.78
98.30
I.loS
86.5
49-80
330-7
J50-7
68.70
96.74
I .Up
79-7
68.10
304-9
205-7
59-69
94-So
I.I40
77.0
97.20
294.4
293.6
50-09
93.62
1.163
69.8
130.7
266.8
395-o
40.31
92-49
1.198
66.0
177-3
252-5
535 -6
32.03
90.07
1.252
57-5
247-7
222 .6
748.5
22.91
83-47
1.294
25-9
334-3
99-2
1010.3
8. ii
75-44
1.376
28.8
429.7
110.3
1298.0
. 7-77
35-n
1. 4*9
553-*
o.o
1673.0
o.o
o.o
Tables of results are also given for 15°, 30°, and 47°.
SOLUBILITY OF MIXTURES OF BARIUM NITRATE AND POTASSIUM NITRATE IN WATER.
(Findlay, Morgan and Morris, 1914; Foote, 1904.)
Gms. per 100 Gms. Sat. Sol. ' Solid
Ba(NO3)2.
6.62
5-49
3-04
2.04
n-39
8.18
8.08
8.42
5-85
5.02
3-02
1.77
O
24.77 b * Results by Foote.
a = Ba(NO3)2, 2b.a = 2KN03.Ba(NO3)2, b = KNO3.
SOLUBILITY OF MIXTURES OF BARIUM NITRATE AND SODIUM NITRATE IN WATER.
(Coppadoro, at o°, 1912; at 30°, 1913.)
Results at o°. Results at 30°.
Ba(NOs)2.
KNOs. Phase.
9.1 6
•25
0
a
9.1 4
.20
8
•15
0+26.0
9-
I
.98
12
.02
26.0
9-
0
.98
16
.80
6+26.0
9-
0
16
.76
6
21.
8
.46
o
a
21.
7
•47
2
.12
"
21. 1 6
•35
5
.98
«
21. 1 6
.06
8
•47
"
2i. i 5
.98
13
.24
0+26.0
21. i 3
.35
18
.24
26.0
21. 1 2
-30
21
•47
"
21. 1 I
.76
24
.86
6+26.0
t°.
25*
25
25
25
35
35
35
35
35
35
35
35
35
Gms. per 100 Gms. Sat. Sol.
KN03.
14-89
16.30
21.99
27.76
O
12.99
17.48
19-75
24
26.05
34.87
34.98
35-01
Solid
Phase.
0+26.0
zb.a
«
6+26.0
0+26.0
26.0
6+26.0
6
21. I
Gms. per loo^Gms. Sat. Sol.
Ba(NO3)2. NaNCb.
33
Solid Phase.
Ba(NO3)2
4.33 0.41
3.34 1.68
2-50 3-54
I. 60 8.02 "
1.56 12.71 «
1.53 20.24
1.56 27.74
i-55 30.81
1.49 35.83
1.55 40.85 98 %Ba(NOs)2+ 2 %NaNO3
1.55 41.3° 26 % " + 73-8% "
1.54 42.06 2.6% " +97-4% "
0.51, 41.68 o % " +ioo % "
Gms. per 100 Gms. Sat. Sol
Solid Phase.
Ba(NOs)2.
NaNOs.
10-33
0
Ba(NOs).
8.58
2-33
"
5-28
7.09
•
3.89
12.07
•
3-54
14.41
"
3.20
17.87
H
3-07
19.06
ii
2.81
23-55
"
2.27
41 .22
"
2. II
48.22
Ba(N03)2+ NaNOs
I
48.50
NaNOs
9
49.16
"
117 BARIUM NITRATE
SOLUBILITY OF BARIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT 30°.
(Masson, 1911.)
Cms, per 100 cc. Sat. Sol. Gms. per 100 cc. Sat. Sol.
P ' HNOa. Ba(NOs)2. HNO3. Ba(NO»)"t.
1.0891 o 54-31
1.0811 8.303 30.50
15.72 27.73
1.0663 31.49 22-76
1.0619 47 .18 19 .71
1.0609 63 17-84
•0633 78.54 16.66
.0668 98.40 15.88
.0783 125.9 14.99
.1050 188.6 14.11
.1341 251.6 13.75
•1645 315.7 13.52
Fusion-point curves (solubility, see footnote, p. i) are given by Harkins and
Clarke, 1915, for the following mixtures:
Ba(N03)2 + NaN03 + KNO3, Ba(NO3)2 + NaNO3, Ba(NO3)2'+ KNO3,
Ba(N03)2 + LiN03, Ba(NO3)2 + LiNO3 + KNO3.
SOLUBILITY OF BARIUM NITRATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL AT 25°.
(D'Ans and Siegler, 1913.)
Gms. C2H6OH Gms. per 100 Gms. Sat. Sol. Gms. CtHsOH Gms. per 100 Gms. Sat. Sol.
^SS^ST 'OaOH. " BatNOa),: ^sS^T ckoH. * Ba(NO3)Z.
o o 9.55 58 57 1.85
10.25 9.5 7.63 78.7 78.2 0.62
18.6 17.5 6.02 90.1 89.9 0.18
25-05 23.7 5.25 99.4 99.39 0.005
40.2 38.3 3.53
Data are also given by Vogel (1903), but'as the results are given in gms. per 100
cc. and densities are omitted, no exact comparison can be made with the above.
SOLUBILITY OF BARIUM NITRATE IN AQUEOUS PHENOL SOLUTIONS
AT 25°.
(Rothmund and Wilsmore — Z. phyisk. Chem. 40, 620, 'oa.)
G. Mols. per Liter.
Gms. per Liter.
G. Mols. per Liter.
Gms. j>er Liter.
CflHfiOH Ba(N03)2.
o.ooo 0.3835
0.045 °-3785
0-082 0.3746
0.146 0.3664
QHsOH. Ba(NO3)2.
0.0 100.2
4.23 98.97
7-7i 97-95
13-73 95 -81
C6H6OH. Ba(N08)2.
0.310 0.3492
O-4OI 0.3400
0.501 0.3299
0.728 (sat.) 0.3098
CoHcOH. Ba(NO3)a.
29.12 91.31
37-73 88.90
47.11 86.26
68.45 81.00
Data for the above system are also given by Timmermans (1907).
100 gms. hydroxylamine dissolve 1 1.4 gms. Ba(NO3)2 at i7°-i8°. (de Bruyn, 1892.)
100 cc. anhydrous hydrazine dissolve 3 gms. Ba(NO3)2 at room temp.
(Welsh and Brodersen, 1915.)
100 gms. methyl alcohol dissolve 0.5 gm. Ba (NO3)2 at 25°. (D'Ans and^Siegler. 1913.)
100 gms. acetone dissolve 0.005 Sm- Ba(NO3)2 at 25°.
BARIUM NITRITE Ba(NO2)2.H2O.
SOLUBILITY IN WATER.
(Oswald, 1914; see also, Vogel, 1903-)
t°. Gms. Ba(N02)2 ^ ... Gms.
— 1-7 9-2 Ice 20 40.3 Ba(NOi)j.HiO
- 3-2 19-5 " 43 50-3
- 5.8 33.1 •• 61 58-6
— 6.5 34.5 " +Ba(NOl)i.H20 80 67.3
— 4.3 34.9 Ba(NOJ)».HlO 92 71.7
+ 17 40* •* no 82
* d of the sat. solution = 1.4897.
BARIUM NITRITE
118
SOLUBILITY OF MIXTURES OF BARIUM NITRITE AND SILVER NITRITE IN
WATER AT 13.5°. (Oswald, 1914.)
Cms. per 100 Gms. HjO.
Ba(NO,),. ' AiNO?. S°Ud Phase"
64 10.2 AgN02+BaAg2(N02)4.H2O
75-6 9-5 Ba(N02)2+BaAg2(N02)4.H20
SOLUBILITY OF BARIUM NITRITE IN AQUEOUS ALCOHOL SOLUTIONS AT
I9.5°-20.5°. (Vogel, 1903.)
% alcohol in solvent: 10 20 30 40 50 60 70 80
184 13.3 9.1 4.8 2.7 0.98
Gms. Ba(N02)2.H20 j
per 100 cc. sat. soli49'3 29*3
BaC2O4.
90
o
BARIUM OXALATE
SOLUBILITY OP THE THREE HYDRATES IN WATER.
(Groschuff — Ber. 34, 3318, '01.)
BaC2043*H20.
BaC2O4.2H2O.
BaC2O4.}H2O.
t°. Gms.BaC2O4 G.M.BaC2O4
per per 100 Mol.
Gms. BaC2O4
per
G. M. BaC2O4
per 100 G. M.
Gms.BaC2O4
per
G. M. BaC204"
per loo Mol.
1000 g. Sol.
H20.
looo g. SoL
H2O.
looo g. Sol.
H20.
O
0.058
O.OOO46
0-053
O.OOO42
0.089
O.OOO7O
9-5
0.082
O.OOO66
. . .
18
O.II2
0.00090
0-089
O.OOO7I
O.I24
0.00099
3°
0.170
O.OCI36
O-I2I
0.00097
0.140
0-OOII2
40
O.I52
O.OOI22
O.I5I
O.OOI2I
45
0-169
0.00135
50
...
...
0.164
O.OOI3I
55
...
O.2I2
0.00170
00
0-175
0.00140
65
...
o 250
O.OO2OO
73
...
0.285
0.00228
75
...
...
0.188
O.OOI5I
90
...
...
...
...
0.200
0.00100
100
...
• *.
• ..
* ...
O.2II
o 00169
The following additional data for the solubility of the above three hydrates in
water are given by (Kohlrausch, 1908). i
BaC2O4.2H20.
BaCi-CMHzO.
' t»
Gms. per Liter.
* t°.
Gms. per Liter.
' t°.
Gms. per Liter.
2.07
0.0553
3
0.0519
0.08
0.0499
4.2
0.059
5-47
0.0575
2.46
0-053
16.1
0.0962
11.28
0.0693
9.62
0.0619
17.8
0.1047
17.9
0.085
15.04
0.0699
23-3
0.0987
17-54
0.0751
28.4
O.II24
27.02
0.091
33-73
O.IOlS
Cantoni and Diotalevi (1905) obtained higher results than either of the above.
SOLUBILITIES OF BARIUM OXALATE (BaCzO4.iH2O) IN AQUEOUS ACETIC ACID AT
26°-27°. (Herz and Muhs, 1903.)
Normality G. Residue* Gms. per IOQCC. Solution. Normality
of Acetic
Acid.
per 50. 05 cc.
CH3COOH
Ba
* Oxalate.
of Acetic
Acid.
0
0.0077
O
.00
0
.0154
3-85
O
•565
0.0423
3
•39
0
.0845
5-79
I
.425
o 0520
8
•55
0
.1039
I7-30
2
•8S
0.0556
17
.11
0
.1111
, • Dried at 70°.
G. Residue* Gms. per 100 cc. Solution
^Sof."' CH3COOH. BaOxalate
0.0564 23.12 O.II27
0.05II 34-76
0.0048 103.90
O 1021
o 0096
119 BARIUM OXALATE
BARIUM AOID OXALATE BaC2O4.H2C2O4.2H2O.
SOLUBILITY IN WATER.
(Groschuff.)
f. '
jms.per K
x> Gms. Solution. Mols. per too Mols. H2O.
Mols. HaCtO*
per i Mol.BaC2O4.
HjC2O4
iC_O4.
H2C204.
BaC204.
o
0.27
O
.030
0.054
0.0024
22
18
0.66
O
.070
0.130
0.0056
24
20.5
0.76
0
.076
0.15
0.0061
25
38
1.61
0.16
o-33
0.013
25
4i
1.82
o
.18
o-37
0.015
25
53
2.92
0
•31
0.60
0.026
24
60
3.60
o
.40
0-75
0-033
22.
5
80
6.21
o
.81
i-34
0.070
J9
90
7.96
I
.11
0.098
18
99
10.50
1
•55
2-39
0.141
17
BARIUM OXIDES.
Data for the lowering
mixtures of BaO and B2(
r of the fusion
33 are given by
points (solubility, see footnote, p. i), of
Guertler (1904). Results for mixtures of
BaO and
CaCl2
and for
BaO and SrCl2
are given
by Sackur (1911-12).
BARIUM Glycerol PHOSPHATES.
SOLUBILITY IN WATER.
Gms. Anhy-
t°. Compound. Formula. drous Salt per Authority.
loo Gms. Sat. Sol.
21 Barium Glycerolphosphate BaCsHrOsP.HzO 4.5 (Rogier and Fiore, 1913.)
13 " a Glycerolphosphate BaCsHrOsP 1.4 (King and Pyman, 1914.)
12 ft BaCaHvOsP.IHzO 5.8 " " " .
21 Glycerolphosphate BaCaHeOeP.^HzO 8.4 (Langheld and Oppmann, 1912.)
22 " di Glycerolphosphate ____ 3.76
BARIUM PICRATE. Solubility in H2O + C2H6OH at 25°. (Fischer, 1914.)
BARIUM PROPIONATE Ba(C3H5O2)2.H2O, also 6H2O.
SOLUBILITY IN WATER.
(Krasnicki — Monatsh. Chem. 8, 597, '87.)
Gms. Ba(C3H5O2)2 Gms. Ba(C3HfiO2)2
t». per IPO Gms. $°. per 100 Gms.
Water. Solution. Water. Solution.
o 47 -98 32-4i 5° 62 -74 38-57
10 51-56 34-02 60 64.76 39 .31
20 54-82 35.42 70 66.46 39.93
3o 57-77 36-65 80 67.85 40.42
40 60.41 37-66 .. ... •••
100 cc. 95% ethyl alcohol dissolve 0.1631 gm. barium propionate at room temp.
(Crowell, 1918 )
BARIUM SALICYLATE Ba(C6H4OHCOO)2.H2O.
100 gms. sat. aqueous solution contain 28.65 g1115- anhydrous salt at 15° and
54.08 gms. at I OO°. (Tarugi and Checchi, 1901.)
BARIUM DinitroSALICYLATE. Solubility in H2O + C2H6OH at 25°.
(Fischer, 1914.)
BARIUM SILICATE BaSiO3.
Fusion-point curves (solubility, see footnote, p. i) for mixtures of:
BaSiO3+CaSiO3 and BaSiO3-fMnSiO3 are given by (Lebedeu, 1911).
BaSiO3+Li2SiO3 and BaSiO3+Na2SiO3 are given by Wallace, 1909.
BaSiO3-j-BaTiOj are given by Smolensky (1911-12).
BARIUM STEARATE 120
BARIUM STEARATE and Salts of Other Fatty Acids.
SOLUBILITY OF BARIUM STEARATE, PALMITATE, MYRISTATE AND LAURATE
IN SEVERAL SOLVENTS. (Jacobson and Holmes, 1916.)
Solvent. t°. Cms. Each Salt (Determined Separately) per 100 Cms. Solvent.
Ba Stearate. Ba Palmitate. Ba Myristate. Ba Laurate.
Water 15.3 0.004 0.004 0.007 0.008
" 50 0.006 0.007 o.oio o.on
Abs. Ethyl Alcohol 16.5 0.006 0.009 0.009 o.oio
50 0.003 0.004 0.004 0.007
Methyl Alcohol 15 o . 042 o . 045 o . 05 7 o . 084
" " 50.5 0.077 0.088 0.108 0.163
Ether 25 o.ooi o.ooi 0.003 0.007
Amyl Alcohol 25 0.007 0.008 0.009 0.009
BARIUM SUCCINATE AND BARIUM ISO SUCCINATE
Ba.CH2CH2(COO)2. Ba.CH3CH2(COO)3.
SOLUBILITY OF EACH IN WATER.
(Miczynski — Monatsh. Chem. 7. 263, 1886.)
Cms. Ba. Succinate Cms. Ba. Iso Succinate
IjO^ per IPO Gms. per iqo Gms.
Water. Solution. Water. Solution.
o 0.421 0.420 1.884 1.849
10 0.432 0.430 2.852 2.774
20 0.418 0.417 3-618 3-493
30 0.393 0.392 4.181 4.014
40 0.366 0.365 4.542 4.346
50 0.337 °-336 4-7oo 4-594
60 0.306 0.305 4-656 4-45°
70 0.273 0.272 4.410 4.224
80 0.237 0.237 3-962 3-8l°
100 gms. H2O dissolve 0.396 gms. Ba Succinate at 18° and 0.410
gms. at 25°.
100 gms. 95% alcohol dissolve 0.0015 gms- Ba Succinate at 18° and
0.0016 gms. at 25°. ' (Partheil and Hiibner — Archiv. Pharm. 241, 413. '03-)
Cantoni and Diotalevi (1905), and Tarugi and Checchi (1901), obtained data
in close agreement with the above.
BARIUM SULFATE BaSO4.
SOLUBILITY IN WATER. (Kohlrausch, 1908.)
One liter of sat. solution contains 0.00115 gm. BaSO4 at o°; 0.0020 gm. at 10°;
0.0024 gm. at 20° and 0.00285 gm- at 30°.
Melcher (1910) obtained results a little lower than the above. His data for
higher temperatures are 0.00336 gm. at 50° and 0.0039 gm. at 100°.
Kohlrausch obtained the following results for the solubility of heavy spar
(BaSO4); 0.0019 gm- at o°, 0.0023 gm. at 10°; 0.0027 gm. at 20°; 0,00315 gm
at 30° and 0.0033 gm. at 33.5°.
100 gms. sat. solution of BaSO4 in 21.37% aqueous ammonium acetate solu-
tion contain O.OI6 gm. at 25°. (Harden, igzG.)
SOLUBILITY OF BARIUM SULFATE" IN AQUEOUS SOLUTIONS OF IRON, ALUMINIUM
AND MAGNESIUM CHLORIDES AT 2o°-25°. (Fraps, 1901.)
Gms. Milligrams BaSO4 per Liter in: Gms. Mgs. BaSO4 per Liter in:
Chloride , ^— , Chloride
Vxiuuiiue /- • • -^ v-mui me s
per Liter. Aq. FeCl8. Aq. AlCla. Aq. MgCl2- per Liter. Aq. FeCl3. Aq. A1C13. Aq.MgCl2-
i 58 33 30 25 150 116 50
2i 72 43 30 5° l6° *7o 5°
5 115 °o 33 ioo 170 175 So
10 123 94 33 ...
121 BARIUM SULFATE
SOLUBILITY OF BARIUM SULFATE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
AND OF NITRIC ACIDS.
(Banthisch, 1884.)
In Hydrochloric Acid. In Nitric Acid.
cc. containing Mgs. BaSO4 Gms. per 100 cc. cc. containing Mgs. BaSO4 Cms. per 100 cc.
i MK Equiv. per i Mg. Equiv. Solution. i Mg.Equiv. per i Mg.Equiv. Solution.
ofHCl. ofHCl. HC1. BaSO/. of HNO3. of HNO3. tiNO3. ' BaSOl.
2. 0.133 1.82 0.0067 2. 0.140 3.15 0.0070
I. 0.089 3.65 0.0089 I. 0.107 6.31 0.0107
0.5 0-056 7-29 o.oioi 0.5 0.085 12. 61 0.0170
0.2 0.017 18.23 0.0086 O.2 0.048 3I-52 0.0241
TOO cc. HBr dissolve 0.04 gm. BaSO4; 100 cc. HI dissolve 0.0016 gm. BaSO4
at the boiling point. (Haslam, 1886.)
SOLUBILITY OF BARIUM SULFATE IN CONCENTRATED AQUEOUS SOLUTIONS OF
SULFURIC ACID AT 2O°.
* (Von Weimarn, 1911.)
Gms. HtSOi per
Gms. BaS04 per
Gms. HzSO4 per
Gms. BaS04 per
ico Gms. Solvent.
100 cc. Sat. Sol.
ico Gms. Solvent.
100 cc. Sat. Sol.
73.83
0.0030
85.78
0.3215
78.04
0.0135
88.08
1.2200
80.54
0.0285
93
. . .*
83.10
O.OSOO
96.17
4.9665
84.15
...t
96.46
18.6900
* Solid Phase = BaSCMIfcSO^.H^ + BaSCU.EkSO*. f Solid Phase = BaSO4 + BaS04.H2S04.H2O.
Data for the above system are also given by Volkhouskii (1910).
100 cc. sat. solution of BaSO4 in abs. H2SO4 contain 28.51 gms. BaSO4, solid
phase = BaSO4.3oH2SO4. (Bergius, 1910.)
100 cc. of sat. solution of BaSO4 in 95% formic acid contain o.oi gm. BaSO4
at 18.5°. (Aschan, 1913.)
Fusion-point curves (solubility, see footnote, p. i) are given the following
mixtures of barium sulfate and other salts:
BaSO4 + NaCl (Sackur, 1911-12.)
+ KC1
+ CaCl2
-f- K2SO4 (Grahmann, 1913; Calcagni, 1912.)
+ Li2SO4 (Calcagni and Marotta, 1912.)
+ Na2SO4 (Calcagni, 1912.)
BARIUM Amyl SULFATE Ba(C5HnSO4)2.2H2O.
SOLUBILITY OF MIXED CRYSTALS OF THE ACTIVE AND INACTIVE SALT IN
WATER AT 20.5°.
(Marckwald, 1904.)
Gms. Salt per Per cent Active Salt Gms. Salt per Per cent Active Salt
ico Gms. H2O. in Dissolved Salt. 100 Gms. HjO. in Dissolved Salt.
28.2 ico 18.3 49.6
26.3 91.6 16.6 36.3
24.8 84.5 15 25.8
21.7 71.2 13.6 10.6
19.5 59.5 12.8 o
Mixed crystals of the active and inactive barium amyl sulfate were dissolved
in water by warming, then cooled to the beginning of crystallization and shaken
two hours at 20.5°. The percentage of the active salt was determined by the
polariscope. Its specific rotation was [a]D= +2.52°.
BARIUM SULFATE 122
BARIUM Isoamyl SULFATE Ba(C5HiiSO4)2.2H2O.
100 gms. H2O dissolve 9.71 gms. of the anhydrous salt at 10°, 11.85 Sms. at
19.3° and 12.15 8mS. at 20.5°. (Marckwald, 1902.)
BARIUM PerSULFATE BaS2O8.4H2O.
100 parts water dissolve 39.1 parts BaS2O8 or 52.2 parts BaS2O8.
4H2O at o°.
(Marshall — J. Ch. Soc. 59, 771, '91**
BARIUM SULFITE BaSO3.
SOLUBILITY IN WATER AND IN AQUEOUS SUGAR SOLUTIONS.
(Rogowicz — Z. Ver Zuckerind. 938, 1905.)
Cone, of Gm. BaSO4 per 100 cc. Sol. ^^ Q{ Gm. BaSO4 per 100 cc. Sol.
S^Sfll. 'at 20°. "TTsoX Sugar Sol. 'at 2o°. "!Ts>.
o° Bx 0.0197 0.00177 40° Bx 0.0048 0.00158
10° 0.0104 0.00335 5°° " 0.0030 0.00149
20° " 0.0097 0-00289 60° " (Sat.) 0-0022 0-OOII2
30° " 0.0078 0.00223
BARIUM SULFONATES.
SOLUBILITY OF SEVERAL BARIUM SULFONATES IN WATER.
Gms. Anhy-
Salt. Formula. f. pj^g.. Authority.
Barium: HzO.
3.4 Diiodobenzene Sulfonate CuHeOek&Ba.H^ 21.5 0.27 (Boyle, 1909.)
2.5 " " CuHeOehSiBa.^H^ 2O 0.522 "
2 Phenanthrene Sulfonate (Ci4H9SO3)2Ba.|H2O 20 0.016 (Sandquist, 1912.)
3 " " (CuH9SO3)2Ba.3H2O 2O 0.03 "
10 (C,4H9S03)2Ba.3H20 2O 0.13
Bromobenzene Sulfonate (CelfcBrSOshBa 17.5 3.31 (Meyer, 1875.)
BARIUM TARTRATE Ba(C2H2O3)2.
SOLUBILITY IN WATER.
(Cantoni and Zachoder — Bull. soc. chim. [3] 33, 751, '05; see also Partheil and Hiibner.)
Gms. Ba(C2H2O3)2
t°. DCT loo cc. t°.
Gms. Ba(C2H2O3)2
per 100 cc.
t".
Gms. Ba(C2H2
per loo cc.
Solution.
Solution.
Solution.
0
O.O2O5
30
0.0315
70
0.0480
10
O.O242
40
0.0352
00
0.0527
20
0.0279
50
0.0389
85
0.0541
25
0.0297
60
0.0440
••
SOLUBILITY OF BARIUM TARTRATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE, SODIUM CHLORIDE AND AMMONIUM CHLORIDE.
(Cantoni and Jolkowski, 1907.)
At Different Temperatures. Varying Concentrations at 16°.
Gms. Ba(C2H2Os)2 per 100 cc. Sat. Sol. in: Gms. Chlo- Gms. Ba(C2H2Oa)2 per 100 cc. Sat. Sol in:
7% KC1.
7%NaCl.
7% NEUC1. Gms. Solvent.
KC1.
NaCl.
NH4C1.
16
O
.0823
0,
,0887
0.1050
o-5
0.0398
0,
,0410
0
.0441
30
0
.1017
0
,1151
0.1370
i
o . 0466
0
0514
o
.0589
55
0
.1230
O
1348
0.1590
3
0.0723
o.
,0826
o
.0892
70
0
.I5OO
O
.1781
o . 2030
10
O.II99
o,
1260.
0
.1342
85
O
.1828
0
.2168
o . 2360
15
0.1435
o,
1440
0
.1585
20
o . 1466
0,
1573
0
•1663
(See Note p. 222.)
123 BARIUM TARTRATE
SOLUBILITY OF BARIUM TARTRATE IN AQUEOUS ACETIC ACID SOLUTIONS AT
26°-27°.
(Herz and Muhs, 1903.)
Normality Cms. residue* Gms. per 100 cc. Solution. Normality. Cms, residue* Gms.per IOQCC. Solution.
01 /vceuc
Acid.
per 50 cc.
Sol.
CH3COOH. Batartratc! ^Atid
L 50 tA..
Sol.
CH3COOH.
Ba tartrate.
O
0.0328
o.
o
•0655
3
•77
o
.1866
22
.62
0.3728
o-565
O.II5I
3-39
0
.2300
5
•65
0
.1865
33
.90
0.3726
1-425
0-1559
8-55
o
•3"5
16
•85
0
.02l8
101
.10
0.0436
2.85
o 1739
17.11
0
•3475
* Dried at 7-°
TOO grams 95% alcohol dissolve 0.032 gm. Ba tartrate at 18° and 0.0356 gm.
at 25°. (Partheil and Hubner.)
BARIUM P TRUXILATE.
100 cc. sat. solution in water contain 0.028 gm. of the salt at 26°. (de'Jong, 1912.)
BEHENIC ACID C2iH43GOOH.
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures of behenic icid and other compounds.
Behenic Acid + Erusic Acid (Mascarelli and Sanna, 1915.)
+ Isoerusic Acid
+ Brassidinic Acid
+ Isobehenic Acid (Meyer, Brod and Soyka, 1913.)
Methylester+Isobehenic Acid Methyl Ester. "
BENZALANILINE CeHsCHiN.CeHs.
Solubility data determined by the freezing-point method are given by Pascal
and Normand (1913), for mixtures of benzalaniline and each of the following
compounds: Azobenzene, benzylaniline, dibenzyl, hydrazobenzene, stilbene and
tolane.
BENZALAZINE C6H5CH : N.N : CHC6H5.
Solubility data determined by the freezing-point method are given by Pascal
(1914), for mixtures of benzalazine and each of the following compounds: Di-
phenylhydrazine, diphenyldiacetylene, naphthalene, furfuralazine, diphenylbuta-
diene and cinnamylidene. Data are also given for mixtures of thiophenylalazine
and cinnamylidene.
BENZALDEHYDE C6H5CHO.
100 gms. H2O dissolve 0.3 gm. C6H5.CHO at room temp. (Fluckinger, 1875; U. S. P.)
Freezing-point data for mixtures of C6H5.CHO and HNO3 are given by Zukow
and Kasatkin (1909).
Para HydroxyBENZALDEHYDE p C6H4OH.CHO.
Freezing-point data are given for mixtures of p hydroxybenzaldehyde + di-
methylaniline and p hydroxybenzaldehyde + phenol. (Schmidlin and Lang, 1912.)
Ortho NitroBENZALDEHYDE o C6H4NO2.CHO.
SOLUBILITY IN WATER AND IN AQUEOUS SOLUTIONS AT 25°.
(Goldschmidt and Sunde, 1906.)
Gms. CelfcNOz. Gms. CelfcNOj. Gms. C«H«NO«
Solvent. CHO per 100 cc. Solvent. CHO per 100 cc. Solvent. CHO per 100
Sat. Sol. Sat. Sol. cc. Sat. Sol.
H2O 0.2316 i raNaCl 0.1899 I wKNO3 0.3199
o.5wHCl 0.2391 2 n " 0.1390 2 n " 0.3419
1 n " 0.2466 o.5nHNOa 0.3207 o.swNaNOa 0.3013
2 n " 0.2658 i n " 0.3758 i n 0.3132
1 nKCl 0.2046 o.5wKNO3 0.3123 2 n 0.3201
2 n " 0.1912
BENZALDEHYDE 124
Meta NitroBENZALDEHYDE m C6H4NO2.CHO.
100 CC. H2O dissolve 0. 1625 gm. m C6H4NO2.CHO at 25° (Goldschmidt and Sunde, 1906.)
" I n HC1 " 0.1813 "
" inKCl " 0.1542 ."
11 2wKCl " 0.1417 "
Para NitroBENZALDEHYDE p C6H4NO2.CHO.
Data for the system p nitrobenzaldehyde + nitrobenzene + hexane are given
by Timmermans (1907).
Solubility data determined by the freezing-point method are given for:
p Nitrobenzaldehyde + Sulfuric Acid (Kendall, 1914.)
m + Benzene (Schmidlin and Lang, 1912.)
m -j- Phenol
BENZALDOXIME C6H6CH:NOH.
Solubility data determined by the freezing-point method are given for mix-
tures of:
a Benzaldoxime + ft Benzaldoxime (Cameron, 1898.)
a Nitrobenzaldoxime + ft Nitrobenzaldoxime. (Beck, 1904.)
BENZAMIDE C6H6CONH2.
SOLUBILITY IN ETHYL ALCOHOL.
(Speyers — Am. J. Sci. [4] 14, 295, '02.)
G.M. Cms. G. M. Cms.
to Sp. Gr. of C6H8CONH2 C6H6CONH2 to Sp. Gr. of C6H6CONH2 C6H6CONHa
* Solutions, per 100 G.M. per 100 Gms. Solutions, per 100 G.M. per 100 Gms.
CaHfiOH. C-sHcOH. C2H6OH. C^OK.
0 °-^33 3-1 8.15 40 0.848 ii .o 28.92
10 0.832 4.2 11.04 50 0.862 14.2 37-34
20 0.833 5.9 15-52 60 0.881 17.2 45-22
25 0.835 6.8 17.87 70 0.913 20.4 53-63
30 0.838 8.2 21.56
SOLUBILITY OF BENZAMIDE IN MIXTURES OF ALCOHOL AND WATER
AT 25".
(Holleman and Antusch — Rec. trav. chim. 13, 294, '94.)
Alcohol.
100
95
90
85
83
80
75
See rematks under a Acetnaphthalide, p. 13.
loo gms. pyridine dissolve 31.23 gms. benzamide at 2p°-25°. (Dehn, 1917.)
100 gms. aq. 50% pyridine dissolve 39.15 gms. benzamide at 2O°-25°.
The coefficient of distribution of benzamide between oil and water is 0.66 at
3° and 0.43 at 36°. (Meyer, 1900, 1909.)
BENZANILIDE.
Solubilities determined by the freezing-point method are given by Vanstone
(1913)- for mixtures of benzanilide and each of the following compounds: ben-
zil, benzylideneaniline, and benzoin.
Results for mixtures of o chlorobenzanilide and p chlorobenzanilide are given
by King and Orton (1911).
Gms.
Gms.
per 100 Gms.
Sp. Gr. of
Solutions.
Vol. %
Alcohol.
QsHsCONHjj
per 100 Gms.
Sp. Gr. of
Solutions.
Solvent.
Solvent.
17.03
0.830
70
23.87
0.925
21 .12
0.856
60
18.98
0-939
24.50
0.878
50
13-74
0.949
26.15
0.895
40
8.62
0.958
26.63
O.9OO
31
5-33
0.967
26.43
0.907
15
2.28
0.982
25 41
O.Qiy
0
i-35
0.999
125 BENZENE
BENZENE C6He.
SOLUBILITY IN WATER AT 22°.
(Herz — Ber. 31, 2671, '98.)
ioo cc. water dissolve 0.082 cc. C6Hfr, Vol. of Sol. — 100.082,
Sp. Gr. = 0.9979.
ioo cc. C6H6 dissolve 0.211 cc. H2O, Vol. of sol. = 100.135,
Sp. Gr. - 0.8768.
SOLUBILITY OF WATER IN BENZENE.
(Groschuff, 1911.)
j.o Gm. HkO per ioo j.° Gms. HsO per ioo
1 ' Gms. Sat. Sol. Gms. Sat. Sol.
3 0-030 55 0.184
23 0.061 66 °-255
40 0.114 77 0.337
BENZENE, AQ. ALCOHOL MIXTURES; BENZENE, AQ. ACETONE MIX-
TURES AT 20°.
H2O added to mixtures of known amounts of the other two and
appearance of clouding noted.
(Bancroft — Phys. Rev. 3, 31, 1895.96.)
C6H6,C2HSOH and H2O C6H6,CH3OH and H2O C6H5, (CH3)2CO and H2O
Per 5 cc.C2H5OH. Per 5 cc. CH3OH. Per 5 cc. (CH3)2CO.
*
cc. H20. cc. C6H6. 'cc. H2O. cc. C6H8.' cc. H2O.
20 0.03 5.0 0.15 8.0 o.io
8 0.13 3.0 0.215 3.0 0.395
4 0-39 2.0 0-59 2.0 0.69
2 1.17 1-4 I.O 1.3 1.0
1.5 1.87 I.o 1-9 O.5I 2.0
i.o 3.57 0.8 3.0 0.295 3.0
0.605 8.0 0.69 4.0 0.2 4.0
0.34 20.0 0.49 8.0 0.15 5.0
C2H5OH added to mixtures of known amounts of CeH6 and H2O until the
solutions became homogeneous at 20°. (Lincoln, 1900.)
Per 5 cc. CsHe. Per 5 cc. CeH6. Per 5 cc. C6H6.
cc. HzO. ' cc. CzHiOH. cc. HzO. cc. CzHsOH. cc. H2O. cc. CzHsOH.' .
I 4-6 20 31.6 50 58
5 12.8 30 41.4 60 65.6
10 19.8 40 39.5 70 73.1
Lincoln also gives results at 10°. Data of a similar character for mixtures of
benzene, ethyl alcohol and water at 20, 25 and 35° are given by Taylor (1897).
For results at 15°, see page 287.
Data for mixtures of benzene, ethyl alcohol and glycerol and for mixtures of
benzene, ethyl alcohol and lactic acid are given by Rozsa (1911).
MUTUAL SOLUBILITY OF BENZENE AND CARBON TETRACHLORIDE.
(Determined by the synthetic method.)
(Baud, 1913.)
to Gms. CeHg per ioo f0 Gms. CsHe per 100 to Gms. C«H« per ioo
Gms. Mixture. Gms. Mixture. Gms. Mixture.
— 24.2 O —40 19.3 —20 48
. —30 2.8 —34 24.2 —io 64.1
-40 8.5 -35tr.pt. 31 o 85.3
— 46.3Eutec. 12.9 —30 36 +5-5 ioo
BENZENE 126
MUTUAL SOLUBILITY OF BENZENE AND CHLOROFORM. FREEZING-POINT
METHOD. (Wroczynski and Guye, 1910.)
Cms. CeH6 « ,. . Cms. C6H6 ~ ,. , Gnfs. CeH6 .
t°. periooGms. **»£ t°. per 100 Gms. pSh°^ t°. per 100 Cms.
Solution. rhase> Solution. Phase- Solution.
— 63.5 O CHCb —60 26.8 C6H« —20 58.3 C6H6
— 70 1 1. 8 " —50 32 " —io 70.8
-75 H-7 " -40 39 " o 88
— 81.7 18.4 CHCU+c6H6 —30 47.8 " 5 100
— 70 22.6 CsH«
The eutectic point was found by extending the curves to their intersection.
The temperature of the eutectic could not be reached by use of liquid CO2.
MUTUAL SOLUBILITY OF BENZENE AND FORMIC ACID. SYNTHETIC METHOD.
(Ennis, 1914.)
t° of Cms. HCOOH t° of Cms. HCOOH per t° of Cms. HCOOH
Miscibility per 100 Gms. Sol. Miscibility. 100 Cms. Sol. Miscibility. per 100 Gms. Sol.
21 9.2 70 31.5 60 74
30 10.3 72 35 40 82
40 12.2 73.2 43-51 20 87
50 16.5 72 60 5 89.6
60 22 70 65
SOLUBILITY OF BENZENE IN AQUEOUS SOLUTIONS OF FORMIC ACID. SYNTHETIC
METHOD. (Ennis, 1914.)
iirr
riCL
iVt. %
(OH.
Gms. CeHj
In 85 Wt. %
HCOOH.
jo Q£ Gms. CeHj
'«H%
yo Q£ Gms. CeHe
In 60 Wt. %
HCOOH.
i t» of Gms. CeHs
Miscibility.
per ioo
Gms. Sol.
Miscibility.
per ioo
Gms. Sol.
Misdbility. G^r gj
Miscibility.
per ioo
Gms. Sol.
57-5
96.3
71
97-5
122
12
105
6
77
94-4
87
96.6
97-5
8-5
82
3-8
95
89.8
101
96
74
6
76
3
112
85-2
100.5
14.3
94-5
24.7
81
IO
80.5
20
46
7
51 12.5
MUTUAL SOLUBILITY OF BENZENE AND ETHYL ALCOHOL. FREEZING-POINT.
METHOD. (Viala, 1914; see also Rozsa, 1911 and Pickering, 1893.)
t o Gms. CeHe per f 0 Gms. CeHe per fo Gms. CeHe per
ioo Gms. Sol. ioo Gms. Sol. ioo Gms. Sol.
-113.9 o -60 19.3 -io 57.6
— ioo 8 —50 24.1 o 85
— 90 io —40 29.8 i 93
- 80 12 -30 37 5.5 ioo
- 70 15 -20 45.7
MUTUAL SOLUBILITY OF BENZENE AND /3 NAPHTHALENE PICRATE,
C6H2(Np2)3OH.CioH7OH. (Kuriioff, 1897.)
Synthetic method used — see Note, p. 16
|.o Gms. Gma. fo Gms. Gms.
Picrate Benzene Picrate. Benzene.
157 ioo. ... 100.0 in. 6 1.173 I-°37 J9-2
148.4 2.128 O.II5 79.3 IO2.O I.oS/ 1.780 II. 2
137.4 1-274 0.170 61.1 29.5 0.390 8.430 0.95
134.2 1-384 0.297 49.3 4.6 1.329 21. 80 0.48
126.8 1.019 0.343 38.3 5.02 ... loo.o
a = Mols. ft Naphthalene Picrate per ioo Mols. of ft Napthalene
Picrate plus Benzene.
Determinations for a large number of isothermes are also given.
127
BENZENE
THE SYSTEM BENZENE, PHENOL AND WATER AT 25°.
(Horiba, 1914.)
In the case of phenol, the bromine method was used for its determination. In
the case of the other two compounds, the amounts required to produce constant
turbidity were measured directly from burettes.
Solubility of Benzene in Aqueous Solu-
tions Containing Phenol and Vice Versa.
Solubility of Phenol in Benzene Solu-
tions Containing Water and Vice Versa.
Saturating
<*«•
Gms. per ioo Gms.
CsHsOH+CeHe+HzO. ^jgj™*
^36-
Gms. per ioo Gms.
IS
CeHiOH.
QHe. *
3s '
UHsOH.
C«H«.
I
.0002
O
0
.198 CeH,
29
,29
0
I
.0008
I
•059
O
. 204
71
63
I
.62
I
.OO2I
2
.602
0
.205
74
5
3
I
.00305
3
.526
o
• 199
I
.0256
69.
,18
16.33
5
•65
0
.17 CoHs+CsHsOH
O
.9891
55<
80
36
•13
5
•953
0
.132 QHsOH
0
.9629
44
39
5o
•56
I
.0059
6
.516
o
•075
0
.9142
21.
15
77
.22
I
.0069
7
• 683
0
.025
o
.8818
4
78
94
.98
I
.0073
8
•195
o
"
0
.8764
0
99
•95
CsHsOH
CeHfiOH+CeH,
CeH.
Data are also given for the solubility of phenol as solid phase, in C6H6 and in
water and in their mixtures. A complete table for the conjugate points, showing
the distribution of phenol between the aqueous and the benzene layers, is given.
The results agree with those of Rothmund and Wilsmore. See page 482.
RECIPROCAL SOLUBILITY, DETERMINED BY FREEZING-POINT METHOD, OF
MIXTURES OFC
Benzene and Phenol.
(Hatcher and Skirrow, 1917.)
Benzene and Pyridine.
(Hatcher and Skirrow, 1917.)
t° of Melting. Ifl*g^*y
«r Solid
;ure. Phase.
t° of Meltine Gms> C<sH? *** Solid
*' ioo Gms. Mixture. Phase.
39-4
O
CeHsOH
-39-4
0
OHsN
30
II. 8
"
-45
IO
"
20
25
"
-50
17
"
10
38.2
"
-55
23-3
"
0
51.5
"
-58Eutec.
26
" +C.H,
— 5.4Eut
ec. 58.4
" +GH8
-5o
31
OH«
- 2.5
67-5
GHa
-40
37-7
"
0
78.3
"
-30
46
<«
+ 2.5
89
"
— 20
57
"
5-i
IOO
"
— 10
7i-5
"
o
90-5
M
Additional
Paterno and
data on the system Benzene + Phenol are given by Dahms, 1895;
Ampola, 1897; Tsakalotos and Guye, 1910, and Rosza, 1911. Add:-
,1 ,T-» IT-» • !• • i T»;_ i : - o~_
SOLUBILITY OF BENZENE IN SULPHUR.
By "Synthetic Method" see Note, p. 16.
(Alexejew, 1886.)
^o Gms. C6Ha per ioo Gms. ^.0
S Layer. C6He Layer i
ioo 6 75 140
no 8 72.5 150
120 10 70 160
Gms. CBHB^per ioo Gms.
S Layer. QHe Layer."
16 6l
I30
12
66
25
164 (crit temp.) 35
55
45
BENZENE 128
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see
footnote, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
Benzene + Benzoic acid (Roloff, 1895. See Benzoic Acid, p. 135.)
" + o Nitrobenzylchloride (Schmidlin and Lang, 1912.)
" -f- Bromoform " "
" -j- Tetramethyldiamino benz-
hydrol
+ Benzhydrol
" + Nitrobenzene (Dahms, 1895.)
+ 0,wand£Chloronitrobenzene)(Bogojawlensky, Winogradow and Bogolubow,
" -f- m Bromonitrobenzene ) (1906.)
" + o, m and p Dinitrobenzene (Kremann, 1908.)
+ Carbon disulfide (Pickering 1893.)
" + Camphene (Kurnakoff and Efremoff, 1912.)
-f- m Cresol (Kremann and Borjanovics, 1916.)
" + Cyclohexane (Mascarelli and Pestalozza, 1907, 1908.)
" + Diphenyl (Washburn and Read, 1915.)
" + Diethylamine (Pickering, 1893.)
" + Diphenylamine (Bruni, 1898; Dahms, 1895.)
" + Ethyl ether (Pickering, 1893.)
" + Ethylene bromide (Dahms, 1895.)
-f- Ethylene dibromide (Baud and Gay, 1911.)
" + Ethylene chloride (Baud and Gay, 1910.)
" -f- Ethylene dichloride (Baud and Gay, 1911.)
" + Menthol (Dahms, 1895.)
" + Methyl alcohol (Pickering, 1893.)
" + Naphthalene r^ad^xlf^5' ****'' ^^^ "^
" + " +j8Naphthol (Bruni, 1898.)
" + + Diphenylamine "
" + Phenanthrene
+ + Carbazol
" + Paraldehyde (Patemo and Ampola, 1891, 1897.)
" + 0, m and p Nitrophenol jCBogojawlensky, Winogradow and Bogolubow,
" + Propyl alcohol (Pickering, 1893.)
+ Quinine (Van Iterson-Rotgans, 1913.)
+ Thiophene (Tsakalotos and Guye, 1910.)
" + Bromotoluene (Paterno and Ampola, 1897.)
" + 1.2.4, 1.2.6 and 1.3.4 Dinitro-L.,
toluene } (Kremann, 1908.)
+ Urethan (Pushin and Glagoleva and Mazarovich, 1914.)
" + p Xylene (Paterno and Ampola, 1897.)
Bromobenzene + Chlorobenzene (Pascal, 1913.)
T lodobenzene "
+ Fluorobenzene "
p Dibromobenzene + 0 Dibromobenzene (Holleman and van der Linden, 1911.)
+ p Dichlorobenzene
-|- p Diiodobenzene (Nagornow, 1911.)
+ p Bromoiodoben- ? „
zene J
| (Bruni and Gorni, l899.)
Chloronitroben- |(pawlewsk. l89g>)
+ m
+ p Bromotoluene (Borodowski and Bogojawlenski, 1904.)
129 BromoBENZENES
SOLUBILITY OF p DIBROMOBENZENE IN SEVERAL SOLVENTS AT 25°.
(Hildebrand, Ellefson and Beebe, 1917.)
Cms. CeH4Br2 (p) Gms. CeffcBn (p)
Solvent. per 100 Gms. Solvent. per 100 Cms.
Solvent. Solvent.
Methyl Alcohol 10.35 Carbon Tetrachloride 36.6
Benzene 83.8 Ethyl Ether 71.3
Carbon Bisulfide 90 Hexane 25.9
DiBromoBENZENE (p} C6H4Br2.
SOLUBILITY IN ETHYL, PROPYL, Iso BUTYL ALCOHOLS, ETC.
(Schroder — Z. physik. Chem. n, 456, '93.)
Determinations by " Synthetic Method" see Note, p. 16.
Grams C6H4Br2 (P) per too Grams Sat. Solution in:
CzHcOH. Crf
O
10
20
30
40
50
60
70
75
80
SOLUBILITY OF MIXTURES OF p DIBROMOBENZENE AND p DICHLOROBENZENE
IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL
Solvent, 50 Vol. % C2H5OH, t = ^.i°. Solvent, 90.9 Vol. % C2H6OH, t = 25°
(Kiister and Dahmer, 1905.) (Kiister and Wiirfel, 1904-05.)
f"LS /~\1X
CsHyOH.
(CHa)CH.CH2OH.
(C2H6)20.
CS2.
C6H6.
\
27
30
34
34
22
38
43
43
29
14
15
47
53
53
36
19
2O
57
62
62
45
26
2?
30
67
72
71
54
38
40
44
77
8!
80
67
576
67
65
87
90
88
79
80-5
85
77
84
94.4
95
94-6
• »
90
Gms. per 100 cc.
Sat. Sol.
Mol. % CeHiBra
in Solute.
Gms. per
loo cc. Sat. Sol.
Mol. % CeHtBra
in Solute.
CeH4Br2.
CeHiCk.
CgHxBrj.
CsHiCh.
0.484
0
100
2.909
0
100
0.505
O.O44
89.8
2.674
0.696
94-3
0.496
0.084
80.7
2.220
2.808
70.7
0.477
0.503
59-3
1.769
4.249
49.1
0.470
0.721
54-4
I.27I
6.237
24-5
0.196
I.3II
ii. 6
0.675
6.877
9.9
O
I .614
0
0
8.271
0
Additional data for the above system are given by Thiel (1903).
Tribrpmo BENZENE, C6H3Br3. Solubility, gms. per 100 gms. at 20-25°:
In H2(X 0.004; in pyridine, 24.3; in Aq. 50% pyridine , 2.01. (Dehn, 1917.)
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see foot-
note, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES.
p Bromochlorobenzene + p Dichlorobenzene (Bruni and Garni. 1899.)
+ 0 Bromochlorobenzene (Holleman and Van der Linden, 1911.)
p Bromoiodobenzene -j- p Diiodobenzene (Nagomow, 1911.)
O Bromonitrobenzene -j- 0 Chloronitrobenzene (Kremann; Kremann and Ehrlich. 1908.)
+ P Bromonitrobenzene (Holleman &deBruyn, 1900; Narbutt, '05.)
m -j- o " (Narbutt, 1905.)
+ p
+ m Chloronitrobenzene (Hasselblatt, 1913; Kuster, 1891.)
-j- m lodonitrobenzene (Hasselblatt, 1913.)
-j- m Fluoronitrobenzene
-j- m Chloronitrobenzene (Kremann, 1908.)
p " -j- p " (Kremann, 1908; Isaac, 1913; Kremann & Ehrlich, 1308.)
ChloroBENZENES
130
ChloroBENZENE C6H5C1.
SOLUBILITY OF CHLOROBENZENE IN SULPHUR.
" Synthetic Method," see page 16.
(Alexejew.)
Grams C6H5Cl^per TOO Grams.
*"• Sulphur
Layer.
QO 13
ioo 18.5
no 27
116 crit. temp.
38
Chlor Ben-
zene Layer.
70
63
53
^DichloroBENZENE, C6H4C12. o and m ChloronitroBENZENE, C6H4C1NO2.
SOLUBILITY OF EACH IN LIQUID CARBON DIOXIDE.
(Biichner, 1905-06.)
o Chloronitrobenzene. m Chloronitrobenzene.
£ 'Dichlorobenzene.
Gms. p C6H4Cl2
t°.
per ioo Gms.
t°.
Sat. Solution.
-33
1.2
-32
— 10
4.2
+ 5
+ 10
II.4
7
20
22.7
8
22
34-4
ii
Gms. o CeH4ClNO2 per ioo
Gms. Sat. Solution.
I
7.8
16 . 5-36 quad. pt.
58.8
65.8
Gms. m C6H4C1NO2
t°. per ioo Gms. Sat.
Solution.
- i 1.8
+ 16.5 II. 2
7.5 38.2quad.pt.
20 53.2
SOLUBILITY OF o, m AND p CHLORONITROBENZENES IN ANILINE, DETER-
MINED BY THE FREEZING-POINT METHOD (see also p. 77).
(Kremann, 1907.)
Gms. Each Compound (Determined Separately) per too Gms. Sat. Sol.
C6H4C1N02.
51.30 ( = 39
69- IS ( = 57
m CeftClNO*.
21.60 (=i4Mol.
31.67 ( = 21.5
49.29 ( = 36.5
P C6H4ClNOz.
27.75(=i8.SMol.%)
31.67 ( = 21.5
38. 50 ( = 27
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see
footnote, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
(Pascal, 1913.)
(Holleman and Van der Linden, 1911.)
(Nagornow, 1911.)
(Van der Linden, 1912.)
Chlorobenzene + lodobenzene
-f- Cyanbenzene
-j- Fluorobenzene
o Dichlorobenzene + p Dichlorobenzene
P "j + p Diiodobenzene
+ p Chloroiodobenzene
1.2.4 Trichlorobenzene + 1.2.3 Trichlorobenzene
+ 1.3-5
+ + i. 2. 3 Trichlorobenzene "
a Hexachlorobenzene + 0 Hexachlorobenzene
p Chloroiodobenzene + p Diiodobenzene (Nagornow. 1911.)
o Chloronitrobenzene -j- p Chloronitrobenzene (Holleman and de Bruyn, 1900.)
-f- (Bogaiawlewsky, Winogradow and Bogolubow, 1906.)
-j- Formic acid (Bruni and Berti, 1900.)
+ m lodoijitrobenzene (Hasselblatt, 1913.)
+ m Fluoronitrobenzene "
-(- Naphthalene (Kremann and Rodenis, 1906.)
-j- Diphenylamine (Tinkler. 1913.)
-j- Naphthalene (Kremann and Rodenis, 1906.)
o lodonitrobenzene + p lodonitrobenzene (Holleman, 1913.)
m Benzene disulf one chloride -{-p Benzene disulfone chloride. (Holleman and Pollak, 1910.)
m
131
NitroBENZENES
MUTUAL SOLUBILITY OF NITROBENZENE AND WATER
(Campetti and Del Grosso, 1913; Davis, 1916.)
Oms r«HiN(
t°.
20
40
00
80
100
120
140
160
Data for the solubility of nitrobenzene in hexane, diisoamyldecane and Ameri-
can petroleum at pressures up to 3000 atmospheres, are given by Kohnstamm and
Timmermans (1913).
SOLUBILITY OF o, m AND p NITROBENZENE IN WATER AND IN PYRIDINE.
(Dehn, 1917.)
Gms. Each Compound Separately per 100 Gms. Solvent.
Solvent.
Gms. CoHsNOi per 100 Gms.
H,O Layer. <
HjHiNOz Layer.
0.19
99.76
0-3
99.6
0.4
99-3
0.8
99
i
98.7
1.3
98.2
1.9
97.2
2.8
95-8
*
H2O Layer.
C«HSN02 Layer.
180
4-2
93-7
200
7.2
91
220
II. 8
87
230
15.8
83
240
23
72
241
26
67
242
32
58
244-5
crit. t. 50.
I
Water 20-25
50% Aq. Pyridine 20-25
Pyridine 20-25
o Nitrobenzene, m Nitrobenzene. p Nitrobenzene.
0.21+ 2.14+ 1.32 +
1 73 two layers formed 85.3
260 . 394 53.2
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see foot-
note, p. i), ARE GIVEN FOR MIXTURES OF NITROBENZENE AND EACH OF THE
FOLLOWING COMPOUNDS:
Ethyl Ether (Tsakalotos and Guye, igro.) Mercuric Bromide (Mascarell and Ascoli, 1907.)
Hexane (Timmermans, 1907, 1911.) Mercuric Chloride
Hexane -f- Resorcine (Timmermans, 1907.)
Isopentane (Timmermans, 1910, 1911.)
Diethyldiacetyltartrate (Scheuer, 1910.)
Menthol
Nitrosobenzene (Jaeger and van Kregten, 1912.)
Phenol (Dahms, 1895.)
Ethylene Bromide "
Naphthalene (Kremann, '04; Kurnakov, etal, '15.)
DiNitroBENZENE (m) C6H4(NO2)2.
SOLUBILITY IN BENZENE, BROM BENZENE AND IN CHLOROFORM.
" Synthetic Method."
(Schroder.)
Gms CaH4(NO2)2 per 100
t° Gms. Sol. in:
15
20
25
30
C6H6
*7 5
26 .o
33 o
40.0
I8.S
23 7
28.7
CHCI3
22 .2
25 o
29.0
33-o
Gms. CflH4(N08)2 per
t°. 100 Gms. Sol. in:
C6Ha
C8H5Br
CHC13.
40
52
.0
38
.0
42
.0
50
62
•5
47
5
52
•5
60
71
.0
57
.0
65
.0
SOLUBILITY OF m DINITROBENZENE IN SEVERAL ALCOHOLS AND ACIDS
(Timofeiew. 1894.)
Solvent.
Gms. m C6H4(NO»)j
t°. per 100 Gms.
Solvent.
Gms.wtCeEUCNCtoj
t°. per 100 Gms.
Sat. Sol.
Solvent.
Sat.
Sol.
Solvent.
CH3OH
13
.8
5.38
5
•65
CHaCOOH
15
•5
15
•7
18.6
C2H5OH
13
.8
2.83
2
.92
t4
23
17
.8
21.6
C3H7OH
13
.8
2
2
C2H5COOH
• 5
12
13.6
C3H7OH
73
43-6
77
•3
"
15
•5
12
•9
14 8
HCOOH
13
•5
9
9
•9
"
23
*3
•45
15-5
HCOOH
•5
9.6
10
• 5
C3H7COOH
13
• 5
7
3
8-3
CH3COOH
13
•5
15-2
X7
•9
"
15
•5
8.
2
8.9
i oo gms. 95% formic acid dissolve 1 1.89 gms. m dinitrobenzene at 20.8°. (Aschan.'is).
100 gms. pyridine dissolve 106.3 Sms. m dinitrobenzene at 2O°-25°. (Dehn, 1917.)
100 gms. 50% aq. pyridine dissolve 45.5 gms. m dinitrobenzene at 2O°-25°. "
NitroBENZENES
132
Solubilities of Di-Nitro BENZENES and of Tri-Nitro BENZENES in
Several Solvents.
(de Bruyn — Rec. trav. chim. 13, 116, 150, '94.)
Grams per 100 Grams Solvent.
Solvent.
(No62)2;
(wz)
(N
o5)a.'
(N
$&§/ <«X*WQ*,
Methyl Alcohol
Ethyl Alcohol
20.5
20.5
3-3°
6.75
3-5
o
o
.69
•4
4-9 (16°) i6.a (15.5°)
1-9(16°) 5.45d5.S0)
Propyl Alcohol
20.5
i
.09
•2
.4
o
298
Carbon Bi-Sulphide
i7.6
0
.236
• i
•35
o
I48
0.25
Chloroform
i7.6
27
. I
32
•4
I,
82
6.1
Benzene
18.2
5
.66
39
-45
a,
56
6.2 (16°)
Ether
17-5
. .
.
1-5
Ethyl Acetate
18.2
12
.96
36
.27
3-
56
Toluene
16.2
3
.62
3°
.66
2.
36
. « •
Carbon Tetra Chloride
16.2
0
• 143
I
.18
0.
12
. • •
Water
(ord.)
0
.014
' o
•0525
0.
008
Symmetrical Tri-Nitro BENZENE.
SOLUBILITY IN AQUEOUS ALCOHOL AT 25°.
(Holleman and Antusch — Rec. trav. chim. 13, 296, '94.)
Vol.%
Alcohol.
G. C6H3(N03)3(*)
per 100 g.
Solvent.
Sp. Gr. of
Solutions.
Vol. %
Alcohol.
G. C6H3(N03)3(5)
per 100 g.
Solvent.
Sp. Gr. of
Solutions.
100
2-34
0-7957
80
o-57
0.8582
95
*-S7
0.8131
75
0-47
0-8708
90
1. 12
0.8288
70
0-37
0.8808
85
0-79
0.8436
60
0.23
0-9064
See remarks under a Acetnaphthalide, p. 13.
100 gms. 93 vol. % ethyl alcohol dissolve 2.1 gms. of o CeH^NC^, 3.1 gms.
m C6H4(NO2)2 and 0.33 gm. p C6H4(NO2)2 at 25°. (Holleman and de Bruyn, 1900.)
loo gms. of each'of the following solvents dissolve the indicated gms. of 1.2.4
trinitrobenzene at 15.5°: C6H6, 140.8 gms.; CHC13, 12.87 gms.; CH3OH, 12.08
gms.; (C2H5)2O, 7.13 gms.; C2H5OH, 5.42 gms; €82, 0.4 gm. (de Bruyn, 1890.)
Data for the solubility of m dinitrobenzene in a solution of nitrobenzene in
hexane are given by Timmermans (1907).
Solubility data, determined by the freezing-point method, are given for mix-
tures of o, m and p dinitrobenzene with fluorene, Kremann (1911); with phen-
anthrene, Kremann, et al (1908). Results for mixtures of o and p dinitrobenzene
with naphthalene, by Kremann and Rodinis (1906). Data for m dinitrobenzene
with nitrotoluenes are given by Giua (1915) and for m dinitrobenzene and diphenyl-
amine by Giua (191 5a). Similar data for mixtures of s trinitrobenzene with
xanthone, quinol, dimethylpyrone, 5 tribromophenol, fluorenone, coumarine,
and phenyl ether are given by Sudborough and Beard (1911). Results for s
trinitrobenzene and 77 dipyridyl are given by Smith and Watts (1910) and for s
trinitrobenzene and fluorene by Kremann (1911). Results for mixtures of m
dinitrobenzene and naphthalene and for 1.3.5 trinitrobenzene and naphthalene
are given by Kremann, (1904) and Kurnakov, Krotkov and Oksman (1915).
BENZYHYDROL (C6H6)2CHOR
Solubility data, determined by the freezing-point method (see footnote, p. i),
are given for mixtures of benzhydrol and phenol and for benzhydrol and di-
methylaniline by Schmidlin and Lang (1912).
133 BENZIL
BENZIL CgHsCO.COCeHs.
Data for the solubility of benzil in aqueous ethyl alcohol are given by Tim-
mermans (1907) and by Kendall and Gibbons (1915). Data for aqueous solu-
tions of benzil and phenol, for benzil and succinic acid nitrile and for benzil and
triethyl amine are given by Timmermans (1907).
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see
footnote, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
Benzil + Dibenzyl (Vanstone, 1913.)
+ Azobenzene
-|- Stilbene "
4- Hydrobenzoin "
-j- Benzoin (Beurath, 1912-13; Vanstone, 1909.)
-j- Benzoic acid (Kendall and Gibbons, 1915.)
BENZINE (Petroleum) C5H12C6H14.
100 parts of alcohol dissolve about 16 parts benzine of 0.638 — •
0.660 Sp. Gr., at 25°.
BENZOIO ACID C6H5COOH.
SOLUBILITY IN WATER.
(Bourgoin — Ann. chim. phys. [5] 15, 171, '78.)
Grams. C6HsCOOH Grams. C«HsCOOH
t<^ per 100 Gms. t°. per 100 Gms.
Water. " Solution." 'Water. Solution.
o 0.170 0.170 40 °-555 0-551
10 0.210 0.209 50 o-775 0.768
20 0.290 0.289 60 I-I55 1-142
25 0.345 0.343 80 2.715 2.643
30 0.410 0.408 100 5-875 5-549
100 grams saturated aqueous solution contain 0.25 gm. C6H5COOH at 15°;
0.3426 gram at 25°; 0.353 gram at 26.4°; 0.667 gram at 45°; 5.875 gms. at
100°.
(Paul, 1894; Noyes and Chapin, 1898; Greenish and Smith, 1903; Hoffman and Langbeck, 1905; Lums-
den, 1905; Philip, 1905; see also Alexejew, 1886; Ost, 1878; Vaubel, 1895; Freundlich and Seal, 1912.)
SOLUBILITY OF MIXTURES OF LIQUID BENZOIC ACID AND WATER.
(Alexejew.)
Determinations by "Synthetic Method," see^Note, p. 16. Figures read from
curve.
Gms. C6H5COOH per 100 Gms. Gms. C6HsCOOH per too Gms.
Aq. Layer. Benzoic Ac. Layer. Aq. Layer. Benzoic Ac. Layer.
70 6 83 ioo 12.0 69.0
80 7.5 79.5 no 18.0 59.0
90 8.5 76 116 (crit. temp.) 35
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF:
(Hoffman and Langbeck.)
Potassium Chloride at 25°. Potassium Nitrate at 25°.
Nor-
mality
Gms.
KC1.
Dissolved C6H5COOH.
Nor-
mality
Gms.
KN03
Dissolved C6H5COOH.
of Aq.
KC1.
per
Liter.
Mol . Cone . Wt . per cent .
of Aq.
KN03
per
Liter.
Mol. Cone
Wt. per cent.
0.02
I.
49
5.0254-IO"4
0.
339
0.02
2.02
5
.0326-10—*
0.340
0.05
-3-
73
4.9801 "
o.
333
0.05
5.06
5
.0421
tt
0.341
O.2O
14.
92
4-7639
o.
322
O.2O
2O .24
5
.0297
K
0.340
0.50
37-
3°
4.3632
O-
295
0.50
5° -59
4
.9400
ft
°-334
I- 00
101.19
4
.7646
"
0.322
BENZOIC ACID
134
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OP:
(Hoffmann and Langbeck.)
Nor-
mality
of Aq.
NaCl.
o.oo
Gms.
NaCl
per
Liter.
0.02
0.05
O-2O
0.50
1. 00
Sodium Chloride.
Gms. C6H5COOH
per 100 Gms. Sol.
at 25°.
0.340
o-339
0-335
o-336
0.282
Sodium Nitrate.
at 45°.
0-667
0.663
0.654
0.617
0.546
0-449
o.oo
1.17
2-93
11.70
29.25
58-50
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF SODIUM
ACETATE, FORMATE, BUTYRATE, AND SALICYLATE.
(Noyes and Chapin — Z. physik. Chem. 27, 443, '98; Philip — J. Ch. Soc. 87, 992, '05.)
Nor-
mality
of Aa
Gms.
NaN03
T)PT
Gms.QHgCOOH
per zoo Gms. Sol.
NaN03.
pel
Liter.
at 25°.
at 45°.
O.O2
1.70
0-340
0.666
O.O5
8-51
0-339
0.663
O.20
17 .02
o-333
0.647
0.50
42-54
0.319
0.613
1. 00
85.09
0.294
Grams
Gram
s C6H5COOH
per Liter of S<
A
Dlution in:
Sodium
Salt per
Liter.
CH3COONa.
HCOONa.
CaH7COONa. C^OH.COONa.
At 26.4°. At 26.4°.
At 25°.
At 26. 46.
At 25°.
At 26.4°.'
0
3-4i
3-53
3-41
3-53
3-53
3-53
I
4-65
4-75
4-25
4-35
4-5o
3-62
2
5-7o
5-85
4-75
4-85
5-40
3-7o
3
6.70
6.90
5.20
5-3o
6-15
3.80
4
7.60
7-85
5-6o
5-70
6.90
3-87
6
8.40
4.00
8
...
4.10
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF SODIUM MONO-
CHLORACETATE, SODIUM SUCCINATE AND POTASSIUM FORMATE AT 25°.
(Philip and Garner, 1909.)
In Aq. (CH2COONa)2.
Gms. per Liter Solution.
(CH2COONa)?. CeHsCOOH".
3-38
4.087
In Aq. CH2ClCOONa.
Gms. per Liter Solution.
CHzClCOONa.' CeHsCOOH.'
3-38
3.684
O
1-375
3.426
6.839
13.710
4.026
4.417
4.929
o
1.182
2.932
5-848
11.730
In Aq. HCOOK.
Gms. per Liter Solution.
HCOOK. 'CeHoCOOH.
3-38
4.087
O
1.025
5.II2
6.564
9.005
5.124
4-734
5-503
The authors also obtained data for the solubility of benzoic acid in aqueous
solutions of sodium acetate and sodium formate which agree closely with those
quoted in the second table above.
ioocc.90%ethylalcoholdissolve36.i gms. C6H5COOHat i5.5°.(Greenish&Smith,'o3.)
100 cc. of a i.o n aqueous solution of aniline hydrochloride dissolve 0.537 Sm-
C6H6COOH at 25°. (Sidgwkk, 1910.)
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL
AT 25°.
(Seidell, 1908, 1910.)
wt. %
C2H8OH
in Solvent.
Sp. Gr. of
Sat. Sol.
Gms. per too Gms Sat.
Sol.
Wt. %
C2H5OH
n Solvent.
Sp. Gr. of
Sat. Sol.
Gms. per 100 Gms. Sat.
Sol.
C2HsOH.
CeHsCOOH. '
C2H6OH. CaHsCOOH.
0
I
O
0.367
60
0-943
45-72
23.80
IO
0.985
9-94
O.OO
70
0.940
49.21
29.70
20
0.970
19.66
1.70
80
0-934
52-8
34
30
0-959
28.83
3-90
90
0.922
57-6
36
40
0.951
36.36
9-IO
IOO
0.908
63-1
36-9
50
0.946
41.50
17
135 BENZOIC ACID
SOLUBILITY OF BENZOIC ACID IN 90% ALCOHOL, IN ETHER AND IN CHLOROFORM.
ABourgoin.)
0 Cms. C6HsCOOH per TOO Grams.
'Solvent. Solution/
90% Alcohol 15 41.62 29.39
Ether 15 31.35 23.86
Chloroform 25 14-30 12.50
SOLUBILITY OF BENZOIC ACID IN SEVERAL ALCOHOLS. (Timofeiew, 1894.)
Alcohol.
Cms. CeHsCOOH per 100 Gm:
-' Alcohol. t°.GmS
CeHsCOOH per 100 Gms.
Sat. Sol. Solvent.
•
Sat. Sol.
Solvent.
Methyl
-18
23.1
3°
Propyl — 18
14-5
16.9
(4
-13
24-3
32.1
-13
15-7
18.5
<(
+ 3
33-5
50-4
+ 3
23.1
30
it
19.2
40.1
67.1
19.2
28.2
39-3
ll
23
4i-7
71-5
23
29.8
42.3
Ethyl
— 18
20.3
25-4
Isopropyl 21.2
32-7
48.5
«
-13
21.2
26.9
Allyl 21.2
25.1
33-4
«
+ 3
28.8
40.4
Isobutyl o
15-3
18
M
19.2
34-4
52.4
Isoamyl 18
2O. 2
25-4
«
23
35-9
55-9
Capryllic 21.2
Ethyleneglycol 18
22.7
8
28.7
8.69
Additional data, agreeing closely with the above, are given by Timofeiew
(1891) and Bourgoin (1878), .,-,'.
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF DEXTROSE.
(Hoffman and Langbeck.)
Normality of Gms. C6Hl2Oa ^solved C^COOH at 25°, Dissolved CeH.COOH at 45*.
Aq. Dextrose, per Liter. Mol. Cone. p^Cent. Mol. Cone. p^St
0.02 3.67 5.0322.10"* 0.34 9-9o88.io~4 0.674
0.05 9-00 5-0403 " 0-34 9-9328 " 0.669
0.204 36-73 5-0303 l( 0.34 9-9323 " 0.669
o-533 96-J5 5-0321 " 0.34 10.0101 ' 0-674
i. 068 192.30 5-0443 " 0-341 10-0369 " 0.676
SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF UREA AND OF THIO UREA.
(Hoffman and Langbeck.)
Normality Gms. CpHsCOOH Dissolved at 25°.
of Solution. per Liter. Mol. Cone. Wt. per cent!
In Aqueous Urea o.io 6.01 CO(NH2)2 5.i876.io~4 0.350
In Aqueous Thio Urea 0.20 15 .23 CS(NH2)2 5-4994 " 0.372
Data for the system benzoic acid, succinic acid nitrile and water are given by
Schreinemakers, 1898, and for the system benzoic acid, phenol and water by
Timmermanns, 1907.
SOLUBILITY OF BENZOIC ACID IN BENZENE AND VICE VERSA. (Roioff, 1895.)
,o Gms. CeHsCOOH per „ ,., p. xo Gms. C«HsCOOHper c ,. . p.
t • ioo Gms. Sat. Sol. Solld Phase' * ' 100 Gms. Sat. Sol. Solld Phase'
5.37 o C6H6 20 8.8 C6H5COOH
5 1-75 30 13
4-50 3-95 50 25
4.20 5 C6H6+C6H5COOH 70 43.5
5 5.05 C6H5COOH 90 64
7 5-50 no 91.5
9 5.70 121 ioo
ii 6
Von Euler and Lowenhamn (1916) found 7.76 gms. C6H5COOH per ioo cc. of sat.
solution in benzene at 25°, and 7.76 gms. C6H5COOH + 2.50 gms. C6H4OHCOOH
o per ioo cc. of benzene solution saturated with both acids.
BENZOIC ACID
136
SOLUBILITY OF BENZOIC ACID IN ORGANIC SOLVENTS.
Gms.
Gms
Solvent.
to CeHsCOOH
per 100 cc. Sat
Sol.
Solvent.
t°.
Sat
Solution.
CsHsCOOH
per loo Gms.
Sat. Sol.
Aq. 75% Acetic Acid
14-16
10.92 (i)
Amyl Alcohol
25
0.875
32.37
(6)
Benzene
14-16
7.04 (i)
Amyl Acetate
25
0.912
22
(6)
Carbon Disulfide
14-16
4-24 d)
Alcohol (Abs.)
25
0.908
58.40
(6)
Carbon Tetrachloride 14-16
4-50 (
i)
Benzene
25
0.897
12.23
(6)
H
25
6.70 (2)
Chloroform
25
1.456
I5-I4
(6
"
26
6.58 (3)
Carbon Tetrachloride 25
1.564
4.l8
(6
Chloroform
25
18.03 (2)
Carbon Disulfide
25
1.282
4.82
(6
Ethyl Ether
14-16
39.80 (i)
Cumene
25
0.906
8-59
(6
Glycerol
15-16
9-07*(4)
Ethyl Ether (Abs.)
25
. . .
46.74
(6)
Ligroin
14-16
0.72 (i)
Ligroin
25
0.720
i-75
(6
Petroleum Ether f
26
0.98 (3)
Naphtha •
25
0.730
2.65
(6
Pentachlor Ethane
25
10.92 (2)
Nitrobenzene
25
1.225
10.05
(6
Tetrachlor Ethane
25
I5-I7
2)
Toluene
25
0.884
10.69
(6
Tetrachlor Ethylene
25
8.06
2)
Spts. Turpentine
25
0.859
5-09
(6)
Trichlor Ethylene
25
13.62
2)
Water
25
I
0.368(6)
it
IS
6-44*(5)
Xylene
25
0.877
9.71
(6)
Dichlor Ethylene
15
9-67*(5)
Gms. CeHsCOOH per 100 gms. sat. sol.
t (B. pt. 30-70.)
(i) Bomwater and Holleman (1912); (2) Herz and Rathmann (1913); (3) de Jong (1909); (4) Ossen-
dowski (1907); (5) Wester and Bruins (1914); (6) Seidell (1910).
One liter sat. sol. of benzoic acid in ethyl acetate contains 8 gms. at —6.5°,
37.7 gms. at 21.5° and 95.7 gms. at 75°. (Lloyd, 1918.)
SOLUBILITY OF BENZOIC ACID IN MIXTURES OF ORGANIC SOLVENTS AT 25°.
(Harden and Dover, 1916.)
Mixtures of Ethyl Ace-
tate + Benzene.
Gms. CeHsCOOH
per zoo Gms.
Solvent.
ii. 6
14
16.5
20
2O.4
22
23-9
Mixtures of Ether
Mixtures of Acetone
+ Chloroform.
+ Benzene.
% CHClj* in
Solvent.
Gms. CsHsCOOH
Solvent.
% CeHo in
Solvent.
Gms. CeHsCOOH
per loo Gms.
Solvent.
100
38.4
100
ii. 6
90
34
QO
18.3
80
30.1
80
24.1
70
26.6
70
31
60
23.2
60
33-5
50
20.8
50
37
40
18.6
40
42.2
30
16.8
30
47
20
15-6
20
49
10
i5-2
IO
Si-3
0
15.0
0
55-6
Solvent.
IOO
QO
80
70
60
50
40
30 26.5
20 29
10 28.2
o 41.2
* This is probably a mistake in the original and should be %(CzHs)£> in Solvent.
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see footnote,
p. i), ARE GIVEN FOR MIXTURES OF BENZOIC ACID AND EACH OF THE FOL-
LOWING COMPOUNDS:
°n CUor0^icA<!d Un^ter and Holler, «£"£» ™^ta* ^
p " "I I9I2>) Salicylic Acid Qaeger, 1907.)
m Nitrobenzoic Acid (Bakunin and Angrisani, 1915.) Succinic Acid Nitrile (Schreinemakers, 1898.)
Benzil (Kendall and Gibbons, 1915.) Sulfuric Acid (Kendall and Carpenter, 1914.)
Camphor (Joumiaux, 1912.) o Toluic Acid (Kendall, 1914.)
Cinnamic Acid (Kachler, 1870; Kendall, 1914.) o Toluidine (Baskov, 1913.)
Dimethylpyrone (Kendall, 1914.) p (Baskov, 1913; Vignon, 1891.)
Fluorobenzoic Acid (Koopal,
137
BENZOIC ACID
DISTRIBUTION OF BENZOIC ACID BETWEEN WATER AND BENZENE:
At 10°.
(Hendrixon, 1897.)
At 20°.
(Nernst, 1891.)
At 25°.
(Farmer, 1903.)
At 40°.
(Hendrixon, 1897.)
Cms. CeHsCOOH
per 100 cc.
Cms. CeHsCOOH
per zoo cc.
Cms. CsHsCOOH per 100 cc.
Cms. CeHsCOOH per
100 CC.
H20.
C«H«
'H2O.
C6H6.
H2O Laver.
C«H6
H2O
CeH« "
Lciycr.
Layer.
Layer.
Layer.
Layer.
Layer.
Lciycr.
0.0215
0.0725
0.0163
0-0535
0.2002
(0.1885*)
3-33S
0.0238
0.0714
0.0412
0.2363
0.0244
0.099
O.2OI2
(0.1891*)
3-329
o . 0404
0.1637
0.0562
0.4422
0.0452
0.273
0.2020
(0.1902*)
3.319
0.0837
0.5740
o . 0890
1.0889
0.0788
0-737
O.H5S
1.0269
0.1215
2.0272
0.1500
2.42
0.1715
2.1420
o . 1409
2.7426
0.2890
9.70
k • •
i
0.2313
3-9167
unionized.
DISTRIBUTION OF BENZOIC ACID BETWEEN BENZENE AND AQUEOUS
POTASSIUM BENZOATE SOLUTIONS AT 25°.
(Farmer, 1903.)
Cms. CeHsCOOK Qms. CeHsCOOH per liter.
per Liter Aq.
Sol. Aq. Layer. C6H6 Layer.
33-88
33-79
33-71
Gms. Mols.
CeHsCOOK per
Liter Aq. Sol.
O.OOQ3
0.028
0.047
Gm. Mols. CeHsCOOH per Litei
Aq. Layer.
0.01587
O.OIS97
0.01603
CsHe Layer.
0.2776
0.2768
0.2762
1.341 1.937
4.035 1.950
6.774 1.956
DISTRIBUTION OF BENZOIC ACID BETWEEN:
Water and Chloroform. (Hendrixon, 1897.) Water and CC14.
At 40°.
Gms. CeHsCOOH per too cc.
At 10'
Gms. CsHsCOOH per too cc.
H2O Layer.
O.O2O8
CeHe Layer.
0.0880
(Seidell, igioa.1)
At 25°.
Gms. CeHsCOQH per 100 cc.
HzO Layer. CCU Layer."
0.134 0.830
0.291 4.41
CeHe Layer. H:zO Layer.
O.O9I5 0.0258
0.0269 0.1518 0.0432 0.2059
0.0327 0.2170 0.0885 0.6961
0.1057 2.0930 0.1553 2.0435
The coefficient of distribution of benzoic acid between olive oil and water at
25° is given by Boeseken and Waterman (1911) as 12.6.
AminoBENZOIC ACID (o) C6H4.NH2.COOH.
SOLUBILITY OF o AMINOBENZOIC ACID IN WATER.
(Lunden, 1905-06.)
Sp. Gr. Gms. C6N4NH2COOH(o)
Sat. Sol. per 100 cc. Sat. Sol.
25
26.1
28.1
0.999
0.519
0-540
0.570
t°.
Sp. Gr.
Sat. Sol.
Gms.
CeH4NH2COOH(0)
per 100 cc. Sat. Sol.
34-9
0.998
0.731
35
0.997
0.744
39-8
0.997
0.889
SOLUBILITY OF AMINOBENZOIC ACID IN AQUEOUS SALT SOLUTIONS AT 25°.
(Lunden, 1905-06.)
Gms.
Normality of Salt
Solution.
SPo<*r- CeH4NlScOOH(0) Normality of
Solution.
0.768 iBa(N03)2
0.507
0.3427
0.1780
0-IS4S
1.080
1.052
1.037
1.018
1.015
Sat. Solution.
0.634 2.633
0.603 i-372
0.598
1.853
0.946
0.560
0-585
0.555
0.549
lity of
It
ion.
Sp. Gr.
Sat.
Solution.
CeH4NH2-
COOH(o)
per 100 cc.
Sat. Sol.
KNOj
1 I -155
1.083
0.501
0-544
I-°33
0-549
KI
tt
(C
I. 221
I .114
1. 068
0.541
0-559
0-550
The author also gives additional data for aqueous salt solutions at 28.1°.
Additional data for the solubility of aminobenzoic acid in aqueous salt solu-
tions are given by Euler (1916).
AminoBENZOIC ACIDS
138
AminoBENZOIC ACID C6H4.NH2.COOH (w).
SOLUBILITY IN WATER AND IN OTHER SOLVENTS.
(de Coninck — Compt. rend. 116, 758, '93.)
In Water.
Gms.
t°. C6H4.NH3.COOH(m)
per 100 cc. HjO.
0
o-43
10
20
30
0.52
0.67
0.87
40
i-i5
SO
60
1.50
2.15
70
3-15
In Organic Solvents.
Gms.
Solvent. t°. C«H4.NH2.COOH(m)
per 100 cc. Solvent.
Ethyl Alcohol (95 °/0 ) 12.5 2.92
Methyl Alcohol (pure) 10.5 4.05
Acetone 11.3 6.22
Methyl Iodide 10-0 0.04
Ethyl Iodide o-o 0.02
Chloroform 12.0 0.07
Bromoform 8.0 trace
MUTUAL SOLUBILITY OF AMINOBENZOIC ACIDS AND WATER AT HIGH TEMPERA-
TURES, DETERMINED BY THE SYNTHETIC METHOD.
(Flaschner and Rankin, 1910.)
Mixtures of m Acid
and H2O.
t° of Gms. m Acid p
Melting. 100 Gms. Mixt
66 crit. sol. temp.
4.8
9.9
18.5
30.6
38
49.4
59-4
69.7
80
87.2
95
100
Mixtures of p acid and
H2O.
t° of Gms. p Acid per
Melting. 100 Gms. Mixture
47 crit. sol. temp.
MIXTURES OF o ACID
and H2O.
t° of Gms. o Acid per
Melting. 100 Gms. Mixture.
83.6
95-8
101.4
103.4
104.4
105
105.6
107.8
112
Il6.2
128.4
144.6
/° reading, for critical saturation and for separating, also given in the case of the
o acid.
Data for the distribution of o aminobenzoic acid between water and benzene
at 25° are given by Farmer and Warth (1904).
77.8
4-6
82.2
5
90
5-8
90
7-1
100
9-7
100
iS-8
no
20.2
105
22
120
51-2
no
32.3
130
73-7
116
SI.8
140
83.7
120
62
ISO
90.7
130
77
160
95-8
150
91.1
170
99-2
170
98
174-4
100
186
100
AminonitroBENZOIC ACIDS C6H3.NO2.NH2.COOH o, m and p.
SOLUBILITY OF THE THREE ISOMERIC AMINONITROBENZOIC ACIDS:
In Ether.
Gms. C6H3.N02.NHj.COOH per
100 cc. Ether.
In Ethyl Alcohol (90%).
Gms. CeH3N02.NH2.COOH per
100 cc. Alcohol.
2.7
5-8
Ortho.
10.84
16.05(6.8°)
Meta.
1.70
Para.
6.41
8.21
3
9.6
Ortho.
8.13
10.70
Meta. Para.
1.79 8.4
2.20 II.3
SOLUBILITY IN WATER OF THE THREE ISOMERIC:
(Vaubel, 1895.)
Aminobenzo Sulphonic Acids. Amino Phenols.
G. qifr.NHt.SOiH^per 100 G. Aq. Sol. o G. CrfMOH) .NH2 per too G. Aq. Sol.
Ortho.
1. 06
Meta. Para.
1.276 0.592(6°)
Ortho.
Meta.
2.6(20°)
Para.
I.I
139 BENZOIC ACIDS
Brom, Chlor and lodoBENZOIC ACIDS.
SOLUBILITY IN WATER AT 25°. (Paul, 1894; Lowenherz, 1898; Vaubel, 1895.)
_ , Per 1000 cc. Aqueous Solution.
Compound. Formula. /— -*- »
Grams. Gram Mol.
Brombenzoic Acid Cel^Br.COOH (ortho) 1.856 0.00924
Brombenzoic Acid CeH4Br.COOH (meta) 0.402 0.00200
Brombenzoic Acid CeHiBr.COOH (para) 0.056 0.00028
Chlorbenzoic Acid CettiCl.COOH (ortho) 2 . 087 o . 01333
lodobenzoic Acid CeKJ . COOH (ortho) 0.952 o . 003 84
lodobenzoic Acid CeKJ.COOH (meta) 0.116 0.00047
lodobenzoic Acid CeELJ.COOH (para) 0.027 (Koopoi, 1912.)
The following results at 28°. (Sieger, 1912.)
Chlorobenzoic acid C^CICOOH (ortho) 2.25
(meta) 0.45
(para) 0.093
MUTUAL SOLUBILITY OF BROMO AND CHLOROBENZOIC ACIDS AND WATER AT HIGH
TEMPERATURES, DETERMINED BY SYNTHETIC METHOD.^FiasdmerandRankin, 1910.)
p Bromobenzoic o Chlorobenzoic m Chlorobenzoic p Chlorobenzoic
Acid + Water. Acid + Water. Acid + Water, j Acid + Water.
j.o Qf Gms. Acid f.0 Qf Gms. Acid ^.0 Qf Gms. Acid *0 nt Gms. Acid
170 (Crit. sol. temp.) IOO .
169 3 102 ,
8 5.5
,7 10
123
123.8
4.2
18.9
167 (crit. t)
162 3
180
6.2
104
20
I42.8(crit.t.)34.3
170
5-4
190
10-5
126
.2(crit. 1034.9
123.8
75-8
180
10
196
27
104
76
125
81.5
183
14-5
2OO
61
no
85.3
130
87.5
184
21.5
210
80
120
92
140
93-2
187.
47
22O
88.3
130
96.5
150
97-5
200
79-5
240
96.9
139
5 loo
156
IOO
220
92
254
IOO
240
IOO
SOLUBILITY OF ORTHOCHLOROBENZOIC ACID IN AQ. SOLUTIONS OF SODIUM ACE-
TATE, SODIUM FORMATE AND POTASSIUM FORMATE AT 25°. (Philip and Garner, 1909.)
In Aq. CH3COONav In Aq. HCOONa. In Aq. HCOOK.
Grams per Liter. Grams per Liter. Grams per Liter.
CHaCOONa.
1.009
2.484
5.027
10.07
CeH4ClCOOH.
3-599
6.181
15.60
18.27
HCOONa.
0.843
2.IO2
4.196
8.410
C6H4C1COOH."
3.381
5.258
7.637
11.02
HCOOK.
0
1.025
2.563
5.124
C6H4C1COOH.
2.128
3.396
5.226
7-543
SOLUBILITY OF CHLOROBENZOIC ACIDS IN SEVERAL SOLVENTS AT 14-16°.
(Bornwater and Holleman, 1912.)
Gms. per 100 cc. Sat. Solution.
Solvent. i -*- — — ^
0C«H4C1COOH. m CoHiClCOOH. p CeH4ClCOOH.
Ligroin 0.07 0.084 trace
Carbon Tetrachloride 0.58 o . 48 o . 04
Benzene 0.92 0.66 0.017
Carbon Disulfide 0.52 0.62 0.016
75% Aq. Acetic Acid 6 . 22 ... 0.32
Ethyl Ether 16 . 96 14 1.72
Acetone 28.42 ... 2 . 58
Ethyl Acetate 13 . 20 ... i . 64
Freezing-point data are given by Bornwater and Holleman (1912) for mix-
tures of o, m and p Chlorobenzoic acids.
BENZOIC ACIDS
140
FluoroBENZOIC ACIDS C6H4FCOOH.
100 cc. aqueous solution saturated at 32° contain 0.882 gm. o
" 0.308 " m
" 0.107 " p
(Slothouwer, 1914.)
lodoBENZOIC ACID p CeHJCOOH.
MUTUAL SOLUBILITY OF PARA IODOBENZOIC ACID AND WATER AT HIGH TEM-
PERATURES DETERMINED BY THE SYNTHETIC METHOD.
(Flaschner and Rankin, 1910.)
t°of
Melting.
175 crit. sol. t.
178
190
200
Gms. Acid per
100 Gms. Mixture.
3
5-8
10
t° of Gms. Acid per
Melting, zoo Gms. Mixture.
207 22
210 41
215 63.5
220 77
t° pf Gms. Acid per
Melting. 100 Gms. Mixture
230 87.4
240 92.7
269 98 . I
270 ioo
p lodo Bromo and ChloroBENZOIC ACID Methyl Esters.
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES.
Qaeger, 1906.)
p Chlorobenzoic methyl ester + p Bromobenzoic methyl ester.
-j- p lodobenzoic
p lodobenzoic " + P Bromobenzoic
HexahydroBENZOIC ACID CH2(CH2.CH2)2.CH.COOH.
ioo gms. H2O dissolve 0.201 gm. of the acid at 15°, d. saturated solution = 1.048.
(Lumsden, 1905.)
HydroxyBENZOIC ACIDS m and p (o = Salicylic Acid, see p. 588).
SOLUBILITY OF META AND PARA HYDROXYBENZOIC ACIDS IN WATER,
BENZENE, ETC.
(Walker and Wood, 1898.)
In Water.
In Benzene.
Gms. CeHvOH.COOH
t°. per ioo Gms. H2O.
Meta.
Para.
10
o-55
0-25
20
0.90
0.50
25
1. 08
0.65
30
i-34
0-81
35
1.64
I .01
40
2.10
1.24
5°
3.10
2.12
00
80
. . .
Gms. CoH4.OH.COOH
Meta.
Para.
O.OOlS
0.008
0.0027
o.oio
0.0035
O.OI2
0.015
0.017
0.028
0.0045
O.OO6O
0.0082
0.0162
0.047
0.028
0.066
In Acetone.
G. CeH4.OH.COOH
per ioo cc. Sol.
Meta. Para.
26.0 22-7
te.
In Ether.
G. C8H4.OH.COOH
per loo^ cc. Sol.
Meta.
9-73
Para.
9-43
ioo gms. sat. sol. in H2O contain 0.7 gm. m acid at 15° and 4 gms. at 50°.
" " " " " " 044 " p " " " "2.98" " "
4i „ „ CH3OH « 53 5g « m « « «
' 236.22 " p ' (Savorro, 1914-)
" 95% formic acid dissolve 2.37 gms. m acid at 20.8°. (Aschan, 1913.)
141
BENZOIC ACIDS
MUTUAL SOLUBILITY OF META AND PARA OXYBENZOIC ACIDS AND WATER AND
OF PARAMETHOXYBENZOIC ACID AND WATER AT HIGH TEMPERATURES, DE-
TERMINED BY THE SYNTHETIC METHOD.
(Flaschner and Rankin, 1910.)
Meta Oxybenzoic Acid
Para Oxybenzoic A
+H20.
+H20.
t°of
Melting.
Cms. Acid per
100 Gms.
Mixture.
t°of
Melting.
Gms. Acid p
loo Gms.
Mixture.
78.2
9-9
77
10
Q0.8
20
90
19.8
98
30
97-4
29-5
103.2
39-8
104.4
40.1
108.8
49
in. 8
50
119.2
60
1 20
59-6
I3I-4
70
134
69.2
143-4
77-9
154-4
80
175-6
90.8
180.6
90.4
199.8
IOO
213
IOO
Para Methoxy benzole
Acid +
H20.
t°of
Melting.
Gms. Acid per'
zoo Gms.
Mixture.
138.2
crit. sol. t.
140
9
142
12
144
18
145
30
146
59-4
150
73-3
160
89.8
170
95-6
184
IOO
Readings for t° of critical saturation obtained by cooling from t° of melting,
are also given by the authors.
Coefficients of distribution of oxybenzoic acids between water and olive oil
are given by Boeseken and Waterman (1911) as follows:] p oxybenzoic acid,
0.6; m oxybenzoic acid, 0.4; 2.4 dioxybenzoic acid, i.o; 2.5 dioxybenzoic acid,
0.3; 3.4 dioxybenzoic acid, 0.05; 3.4.5 trioxybenzoic acid 0.025.
MethylBENZOIC ACIDS C6H4COOH.CH3. o, m, and p.
SOLUBILITY IN WATER.
(Vaubel, 1895.)
Gms. C6H4COOH.CH3 per 1000 Gms. Sat. Solution.
25
Ortho
1.18
Meta.
0.98
Para.
o-35
NitroBENZOIC ACIDS C6H4.NO2.COOH. o~m, and p.
SOLUBILITY IN SEVERAL SOLVENTS.
(de Connick, 1894; for solubility inHzO, see also Paul; Vaubel; Lowenherz; Goldschmidt, 1898; Holle-
man, 1898; Noyes and Sammet, 1903; Sidgwick, 1910.)
Gms. CeH4.NO2.COOH per 100 cc. Solvent.
Ortho.
Meta.
Para.
""*
Water
15
0
-625
0.
238
0
.0213
tt
20
o
.682
(o.
645G.)
o.
315
o
•039
"
25
0
.738
(o.
779G.)
o.
341
0
.028(0.
045)
tt
30
0
.922
(o.
922G.)
it
35
I
.141
(i
054)
0.
477
o
.0419
Methyl Alcohol
10
42
.72
47-
34
9
.6
Ethyl Alcohol
IO
28
.2
33-
1(11.7°)
o
•9
" (abs.)
15
37
.58*
47-
26*
XQ
.71*
" (33Vol.%)
15
o
.64 (ll.
8°)
o.
52
O
•055
Acetone
10
41
• 5
41
5
4
•54
Benzene
IO
0
.294
0.
795
0
.017(12..?°)
Carbon Bisulfide
10
0
.OI2
o.
10(8.5°)
o
.007
Chloroform
10
15
0
i
•455
.o6f
(n
°)
5-
3-
678
4St
o
o
.066
.o88f
"
25
i
-i3t
4-
o
•H4t
M
35
i
•59t
3Jt
0
Ether
10
21
•58
25-
175
2
.26
Ligroin
IO
trace
0.
013
0
Gms. acid per 100 cc. saturated solution. f = Gms. acid per 100 gms. solvent.
NitroBENZOIC ACIDS
142
SOLUBILITY OF ORTHO NITROBENZOIC ACID IN WATER. (Noyes and Sammet, 1903.)
C6H4N02COOH o per Liter Sol. ^ CelfrNChCOOH o per Liter Sol.
Millimols. Grams. Millimols. Grams.
10 26.62 4.645 25 43.3 7.231
15 31-06 5-187 30 51.6 8.616
20 36.57 6.106
Additional determinations by other investigators, in millimols C6H4NO2COOH
o per liter at 25°, are: 46.5 (van Maarseveen, 1898); 44.19 (Paul, 1894); 42.3
(Holleman, 1898); 43.6 (Kendall, 1911).
SOLUBILITY OF ORTHO, META AND PARA NITROBENZOIC ACIDS IN WATER
AT HIGH TEMPERATURES, DETERMINED BY THE SYNTHETIC METHOD.
(Flaschner and Rankin. 1910.)
o C6H4NO2COOH+H*O. m C6H4NO2COOH+H2O. p C6H4NO2COOH+H2O.
to t
Gms. Acid
t° of:
Gms. Acid
to -f
Gms. Acid
Of
per zoo Gms.
per 100 Gms.
Sat. Sol.
OI
Melting.
per 100 Gms.
Sat. Sol.
Melting.
Solution'
52 crit. t.
. . .
63.2
2
118 crit.
t.
69
5
77-4
6
143
5
75
9.9
77-4
90
7
150
9
78
13-5
77-4
100
10.5
155
14-5
79
49-5
77-4
105
17
1 60
30
80
62
77-4
107 . 5 crit.
t. 30
165
53-5
85
73-5
77-4
106
So
170
65-5
90
78.6
77-4
100
58.6
180
76.7
100
83.5
77-4
90
65-4
190
83-2
120
94
80
74
200
88
I48
100
100
. . .
88.5
220
J 95-2
120
96.8
237
100
140.4
100
Data for the solubility of mixtures of o, m and p nitrobenzoic acids in water at
24.4° are given by Holleman (1898).
SOLUBILITY OF ORTHO NITROBENZOIC ACID IN AQUEOUS SOLUTIONS OF HYDRO-
CHLORIC, FORMIC, MALONIC AND SALICYLIC ACIDS AT 25°. (Kendall, 191 ij
Gms. o
Normality CeHUNCfe.COOH
of Solvent. per Liter Sat.
Solution .
7.28l
7.144
6-934
Solvent.
Normality
of Solvent.
HC1
Gms.
C6H4Np2COOH
per Liter Sat.
Solution.
Solvent.
HCOOH
0.0179
0-0357
0.125
0.250
0.500
0.0517
o . 0998
6.146
5-66i
4.976
4-997
4.752
7.188
7.124
CH2(COOH)2
C6H4(OH)COOH
o
0.0313
O.IOOI
0.2004
0.0094
0.0136
0.0162
6.656
7.276
7-352
7-369
SOLUBILITY OF ORTHO NITROBENZOIC ACID IN AQUEOUS SOLUTIONS OF
DEXTROSE, SODIUM CHLORIDE, AND OF SODIUM NITRATE.
Original results in molecular quantities. (Hoffman and Langbeck, 1905).
In Dextrose. In NaCl. In NaNO3.
G.QH1208 G.(0)C«H4N02.COOHG.NaCl. G.^C^NOa-COOH G.NaNO8 G.^CeEUNOz-COOH
i*r TOO cc. per 100 g. Solvent, per I00 cc. per 100 g. Solvent. pgr IOO cc. per 100 g. Solvent.
Solution.
At 25°. j
M 35b.
Solution.
At 25°.
At 35°-
Solution.
At 25°. i
Vt 35*.
0-0
0.736
-063
O.II7
o-743
I .072
O.I7O
0.746
.074
0.36
0-736
.064
0.195
0.746
I .075
0.284
o-754
.080
1. 80
0.732
.061
0.585
0.749
I .070
0.851
0.767
.096
9-50
0.722
.051
2.425
0.688
0.967
4-255
o-774
.097
20-00
0-703
•030
S.8o
0-597
0.831
8.510
0.748
•047
143
NitroBENZOIC ACIDS
SOLUBILITY OF ORTHO NITROBENZOIC ACID IN AQUEOUS SOLUTIONS OF
SODIUM BUTYRATE, ACETATE, FORMATE, AND SALICYLATE AT 26.4°.
(Philip, 1905.)
Original results in terms of '- per liter.
100
Gms. Na Salt
o-ms. \jn
.iiu v^n^v^^JLi.
i.>* v/2 l-'C1 Jt-*itci UJ
per Liter.
C3H7COONa.
CH3COONa.
HCOONa.
C6H4.OH.COONa.
0
7-85
7-85
7-85
7-85
0-5
8-35
8.50
8.60
8-35
1.0
8.90
9.15
9-50
8.70
2
10. 0
IO.8o
n-5
9-4
3
II. 2
12-55
13 .5
II. 0
4
12-4
14-5
15.6
11.5
6
15.2
Solvent.
CH3OH
<(
C2H5OH
SOLUBILITY OF ORTHO NITROBENZOIC ACID IN SEVERAL ALCOHOLS.
(Timofeiew, 1894.)
Gms. Acid per 100 Gms. Gms. Acid per 100 Gms
Sat. Sol. Solvent. i Sat. Sol. Solvent.
56.6 C3H7OH o 17.7
I09.I " 22 31.2
(CH3)2CH.CH2OH o
o
22
O
22
36.2
52.2
23-3
42.7
30-4
74-5
9-65
21.5
45-5
10.7
Freezing-point data for mixtures of o nitrobenzoic acid and dimethylpyrone are
given by Kendall (i9i4a).
SOLUBILITY OF META NITROBENZOIC ACID IN SEVERAL ALCOHOLS.
Solvent.
CH3OH
C2H5OH
(Timofeiew, 1894.)
^0 Gms. Acid per 100 Gms.
Solvent.
C2H5OH
C3H7OH
^0 Gms. Acid per 100 Gms
0
19
Sat. Sol.
41-9
53-7
Solvent.
72.2
116
21-5
0
Sat. Sol.
43-9
24.1
Solvent.
89.8
31-8
21.5
0
57-i
33-6
I33-I
50.6
tt
19
21.5
32.5
45
48
19
42-3
73-2
SOLUBILITY OF META NITROBENZOIC ACID IN AQUEOUS SOLUTIONS OF SODIUM
ACETATE, SODIUM FORMATE, SODIUM MONOCHLORACETATE AND POTASSIUM
FORMATE AT 25°.
(Philip and Garner, 1909.)
In CHsCOONa.
Gms. per Liter.
In HCOONa.
Gms. per Liter.
In CH2ClCOONa.
Gms. per Liter.
In HCOOK.
Gms. per Liter.
CHs-
COONa.
m CeH4N02-
COOH.
HCOONa.
m C6H4NOr
COOH.
CH2C1-
COONa.
m CeH4NO2-
COOH.
HCOOK.
m\. COOH.
O
I.OO9
2.484
5.027
10.07
5-144
7.932
12. 6l
20.77
0
0
2
4
8
.843
.102
.196
.410
3.424
4.776
6.380
8.616
11.90
0
1-375
3.426
6.839
13.710
3
4
4
5
7
.424
•075
.876
.861
.264
0
I .
2.
5.
025
563
124
3
4
6
8
.424
.742
.446
•5Si
NitroBENZOIC ACIDS 144
SOLUBILITY OF PARA NITRO BENZOIC ACID IN AQUEOUS SOLUTIONS
OF ANILIN AND OF PARA TOLUIDIN AT 25°.
(Lowenherz — Z. physik. Chem. 25, 395, '98.)
In Anilin. In ^-Toluidin.
G. Mols. per Liter. Gms. per Liter. G. Mols.^per Liter. Gms. per Liter.
HoNH" %oS" ^^H'-(aX)H2' CCH3NH*~ SoH02'
CH3.
CfiHtNO,.'
COOH.
D.O
O
.00164
o.o
0
.274
0
.0
0.00164
O
.0
0.274
D.OI
O
.00841
0.91
I
.406
0
.01
O-OIOO
I
.071
I .671
D.02
0
.01379
1.82
2
•3°4
o
.02
0.0174
2
.142
2 .OX>2
3.04
0
.02172
3-64
3
.629
o
•03
0.0245
3
.213
4-097
3.08
o
•0347
7.29
5
.798
1000 cc. of sat. solution of pira nitrabenzoic acid in aqueous I normal sodium
para nitrobenzoate contain 0.0046 gm. mols. = 0.768 gm. ^Cgl^NC^COOH at
25°. (Sidgwick, igzo.)
SOLUBILITY OF PARA NITROBENZOIC ACID IN SEVERAL ALCOHOLS.
(Timofeiew, 1894.)
Gms. Acid per 100 Gms. Gms. Acid per 100 Gms.
S°1VCnt- * ' 'Sat. Sol.' Solvent.' ^^ * ' Sat. Sol. ' Solvent. '
18.5 3-45 3-57 C2H5OH 21 3.22 3.32
21 3-75 3-90 C3H7OH 18.5 2.12 2.17
C2H5OH 18.5 3.25 3.36 19.5 1.85 1.90
19-5 3-16 3-26 21 2.29 2.34
DinitroBENZOIC ACIDS C6H3(NO2)2COOH. 1.3.5 and 1.2.4.
SOLUBILITY OF 3.5 AND OF 2.4 DINITROBENZOIC ACIDS IN AQUEOUS
SOLUTIONS OF SODIUM ACETATE AT 25°.
(Philip and Garner, 1909.)
Gms. per 100 cc. Sat. Sol. Gms. per 100 cc. Sat. Sol.
CHaCOONa.
3.5C«H,(NOi)jCOOH.
CHsCOONa.
2.4C6H3(N02)2COOH.
0
0.1314
0
0.0572
O.0976
0.3392
0.0976
0.2056
0.2428
0.6720
0.2428
0-3434
0.4846
I.2OI
0.4846
0.5023
0.9718
2.H5
0.9718
0.7440
Data for the solubility of 1.3.5 dinitrobenzoic acid in water and aqueous
solutions of KC1, NaCl, KNOs and NaNOs, and for its distribution between
water and benzene at 25°, are given by B. de Szyszkowski (1915).
SOLUBILITY OF 1.3.5 DINITROBENZOIC ACID IN WATER AT HIGH TEMPERATURES,
DETERMINED BY THE SYNTHETIC METHOD.
(Flaschnw and Rankin, 1910.)
+„ Gms. Acid per *° Gms. Acid per to Gms. Acid per
100 Gms. Sol. 100 Gms. Sol. 100 Gms. Sol.
i23.8crit. t. ... 123 66.5 160 90.9
113 4-4 125 72.7 180 95
120 9.3 130 79-3 200 99
121 14.5 140 85.7 206 100
122 40 150 89
145
NitroBENZOIC ACIDS
SOLUBILITY OF NITROBROMOBENZOIC ACIDS AND OF NITROCHLOROBENZOIC
ACIDS IN WATER AT 25°.
(Holleman, 1910.)
Acid.
C6H3COOH.NO2.Br 1.2.3
C6H3COOH.NO2.Br 1.2.5
Cms. Acid per
100 cc. Sol.
0.033
0.741
Acid.
Cms. Acid per
100 cc. Sol.
C6H3COOH.NO2C1 1.2.3 0.047
C6H3COOH.NO2.C1 1.2.5 0.967
Holleman also gives data for the solubility of various mixtures of the above
two bromo compounds and of the two chloro compounds and' uses the results for
estimating the quantity of each in an unknown mixture.
Dinitro p oxyBENZOIC ACID C6H2OH(NOj)2COOH.
SOLUBILITY OF MIXTURES OF DINITRO PARA OXYBENZOIC ACID AND OTHER
COMPOUNDS IN ABSOLUTE ETHYL ALCOHOL AT 29.6°.
(Morgenstern. 1911 )
Dinitro p Oxybenzoic
Acid -f Phenanthrene.
Dinitro p Oxybenzoic
Acid + Fluorene.
Dinitro p Oxybenzoic
Acid + Retene.
Gms. per
IOC
ems. Gms. per ioo Gms.
Gms. per
ioo Gms.
Sat.. Sol.' C,,.M T>U_ Sat, Sol. Solid
Sat.
Sol.
Solid
Acid.
p]
tl
Sre^e1." AdcL
_„ Phase.
Fluorene.
Acid.
Retene.
Phase
2.0483
O
.1333 Acid 2.0440
0.1232 Acid
2.0232
0
Acid
2.0776
O
.2796 2.0823
0.3484
M
2 . 0484
0.1236
1
2.1249
0
.5267 2.1045
0.4824
w
2-0933
0.3446
'
2.2195
i
• 0311
2.1744
o . 8960
M
2. 1276
0.5162
1
2.2883
i
•4310
2.2618
I . 4308
M
2 . 2346
1.0489
'
1.2171
6
.0092 Phena
threne 1 . 0490
3.8618 Flu<
jrene
2 • 3034
1.3634
1
0.8681
5
.8300
0.8004
3.7566
M
1.9664
3-3698
Retene
0.6017
5
.6890
0.5620
3-6532
w
0.7830
3-0032
"
0.3487
5
.5619
0.3900
•
0-5597
2.9331
"
0.2157
5
.4890
0.2113
3-5024
•
o. 2740
2.8466
"
0
5
.3781
O
3.4II5
O
2.2795
"
BENZOIC ANHYDRIDE (C6H5CO)2O.
Freezing-point data are given for mixtures of benzoic anhydride and sulfuric
acid by Kendall and Carpenter (1914).
BENZOIN (Benzoyl phenyl carbinol) C6H6CH(OH)COC6H5.
SOLUBILITY OF BENZOIN IN WATER, PYRIDINE AND AQUEOUS 50% PYRIDINE
AT 20-25°.
(Dehn, 1917.)
Solvent.'
Water
Aq. 5° % Pyridine
Pyridine
Cms. Benzoin per ioo
gms. Solvent.
o 03
6.63
20.20
ioo gms. 95% formic acid dissolve 3.06 gms. benzoin at 18.5°. (Aschan, 1913.)
Freezing-point data (solubilities, see footnote, p. i) are given by Vanstone
. for mixture of benzoin and each of the following compounds:
Dibenzyl, benzylaniline, benzylideneaniline and hydrazobenzene.
BENZOPKENONE
146
BENZOPHENONE (C6H6)2CO.
SOLUBILITY IN AQUEOUS ALCOHOL AND IN OTHER SOLVENTS.
(Derrien — Compt. rend. 130, 722, 'oo; Bell — J. Physic. Chem. 9, 550, '05.)
In Aqueous Alcohol at 40°.
Wt. % Cms. (C6H6)2CO
Alcohol per 100 Gms.
(BeU.)
Jolveni
'• Solvent.
Solution.
40
2
1.0
45
5
4-8
50
8
8-3
55
II
9-9
60
16
13-8
65
28
22.6
Wt.%
Gms. (CftH6)2CO
Alcohol
per 100 Gms.
in Solvent.
Solvent. Solution.
67-5
39 28.1
70
56 35-9
71
67 39.2
72
90 47.4
72-5
105 51.2
73
156 61.0
In Aqueous Alcohol and other Solvents.
(Derrien.)
Solvent.
Gms. Gms.
£"££ «o,ven, f. £*«»
Solvent. Solvent.
17
13-5
Ethyl Ether (rectifiec
I) 12.7
*7-S
17
3-8
Benzene
17
76.9
17
17
2.2
J-3
Xylene
Nitro Benzene
17.6
iS-8
38-4
58.8
9.8
II
Chloroform (com.)
16.5
55-5
15
14-3
Bromoform
17-3
33-3
9.6
19.2
Toluene
17.2
55-5
16.1
66.6
Ligroine
14.6
6-7
97% Ethyl Alcohol
85 cc. 97% Alcohol + 15 cc. H2O 17
80 " " +20
75 " " + 26
Methyl Alcohol (pure)
« it «
Acetic Ether (pure)
Carbon Disulfide
Determinations made by means of the Pulfrich refractometer (Osaka, 1903-8),
gave 39 gms. benzophenone per 100 gms. absolute ethyl alcohol at 20°, and
78.6 gms. benzophenone per 100 gms. benzene at 25°.
SOLUBILITY OF BENZOPHENONE IN AQUEOUS SOLUTIONS OF PHENOL AND OF
n BUTYRIC ACID, DETERMINED BY THE SYNTHETIC METHOD, ARE GIVEN
BY TlMMERMANS (1907).
In Aq. 71.4% C6H6OH
36.51% C6H5OH
(Sat.
t = 65.3).
(Sat.
t = 20.6).
t°of
Sat.
Gms. (C«Hi)«CO
per loo Gms. Sat.
Sol.
t°of
Sat.
Gms. (C6H5)2CO
per 100 Gms.
Sat. Sol.
75-4
0.685
26.1
0.96
81.1
1. 06
29-3
1.77
85.3
I.4I
39-5
4.06
88.1
1.67
55-5
7.82
82.6
16.82
In Aq. 39.4% C3H7COOH
(Sat. t = -2.3).
t°. of
Sat.
Gms. (C6ft)2C(
per 100 Gms.
Sat. Sol.
6.1
0-439
18.5
1. 12
28.9
I.7I
44
2.66
61.6
3-92
75-2
5-09
Solubility data for mixtures of benzophenone and resorcinol and for benzo-
phenone" and pyrocatechinol, determined by the freezing-point method, are given
by Freundlich and Posnjak (1912). Similar data for mixtures of benzophenone
and thymol are given by Pawlewski (1893). Results for mixtures of benzophenone
and sulfuric acid are given by Kendall and Carpenter (1914).
BENZOYL CHLORIDE, BENZOYL tetra hydro quinaldine, d and /.
Fusion-point data are given for mixtures of benzoyl chloride and phenol by
Tsakalotos and Guye (1910), and for mixtures of the d and / forms of benzoyl
tetrahydroquinaldine, by Adriani (1900).
147
BENZYLAMINES
BENZYLAMINE HYDROCHLORIDE C6H5CH2.NH2.HC1.
IOO gms. H2O dissolve 50.6 gms. of the compound at 25°. (Peddle and Turner, 1913.)
DiBENZYLAMINE HYDROCHLORIDE (C6H5CH2)2NH.HC1.
IOO gms. H2O dissolve 2.17 gms. of the compound at 25°. (Peddle and Turner, 1913.)
loo gms. chloroform dissolve 0.37 gm. of the compound at 25°. '
TriBENZYLAMINE HYDROCHLORIDE (CeHsCH-OsN.HCl.
IOO gms. H2O dissolve o.6l gm. of the compound at 25°. (Peddle and Turner, 1913.)
ioo gms. chloroform dissolve 1 1 .41 gms. of the compound at 25°. '
DiBENZYL C6H5CH2.C6H6CH2, BENZYLANILINE C6H5CH2.NHC6H6.
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see
footnote, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
Dibenzyl+ Stilbene
" + Benzylphenol
" -j- Hydrobenzene "
+ Tolane
Benzylaniline + Dibenzyl "
+ Stilbene
+ Benzylphenol
+ Hydrazobenzene
+ Tolane
NitroBENZYL CHLORIDE p C6H5CHNO2.C1.
SOLUBILITY IN SEVERAL SOLVENTS AT 25°.
Gms. p GiHsCH.NCkCl
Solvent.
(Bruni, 1898: Pascal and Normand, 1903.)
(Pascal and Normand, 1913-)
per ioo Gms.
Solvent.
(v. Halban, 1913.)
Gms. p CsHsCHNOz-Cl
per ioo Gms.
Solvent.
Sat
.Sol.
Methyl Alcohol
8
.87
8
•15
Ethyl Alcohol
7
.10
6
.63
Propyl Alcohol
5
.70
5
•39
Amyl Alcohol
4
.88
4
•65
Butyl Alcohol
21
•5
17
• 7
Acetic Acid
18
.1
15
•3
Acetone
107
5i
•7
Acetophenone
63
.1
38
•7
Paraldehyde
24
•9
19
•9
Ether
23
.1
18
.8
Acetonitrile
96
.6
49
.1
Nitromethane
68
.8
40
.8
o Nitrotoluene
5i
.1
33
.8
Solvent.
Sat. Sol.
57-8
36-4
57-8
36-4
43-3
30.2
51.2
33-9
12.5
10.4
32
24.2
47.6
32-3
6.05
5-69
45-3
31.2
31-7
. 23.4
1.30
1.28
0.49
0.49
69.7
37-4
Nitrobenzene
Ethylacetate
Ethylbenzoate
Ethylnitrite
Isoamylbromide
Brombenzene
Chloroform
Carbon Tetrachloride
Benzylchloride
a Bromnaphthaline
n Hexane
Isopentane
Benzene
Data for the lowering of freezing-point are given by Holleman (1914) for mixtures
of o and p nitro benzylchloride.
DiBENZYL HYDRAZINE C6H6CH2.NH.C6H5CH2NH.
Reciprocal solubilities of dibenzylhydrazine and cinnamylidene, determined by
the method of lowering of the fr.-pt. (see footnote, p. i), are given by Pascal ('14).
ChloronitroBENZYLIDENES C6H6C: N02.C1. BENZYLIDENE NAPHTHAL-
AMINES C6H5CH:NCi0H7.
DATA FOR THE LOWERING OF THE FREEZING-POINTS (solubilities, see foot-
note, p. i) ARE GIVEN FOR THE FOLLOWING MIXTURES.
o Chloronitrobenzylidene -f m Chloronitrobenzylidene (Holleman, 1914.)
p +m
P " +o
a Benzylidene naphthalamine +/3 Benzylidene naphthalamine (Pascal and Normand, '13.)
BERYLLIUM ACETATE (basic) Be4O(CH3COO)6.
ioo gms. chloroform dissolve 33.3 gms. Be4O(CH8COO)6 at 18°. (Wirth, 1914.)
BERYLLIUM FLUORIDE 148
BERYLLIUM Potassium FLUORIDE, etc.
SOLUBILITY IN WATER AND IN ACETIC ACID SOLUTIONS.
(Marignac; Sestini, 1890.)
Gms. Anhydrous Salt
Salt. Formula. Solvent. per 100 Gms. Solvent.
At 20°. At 100°.
Beryllium potassium fluoride BeF2.KF Water 2.0 5.2
sodium " BeF2.NaF " 1.4 2.8
hydroxide Be(OH)2 Water + CO2 sat. 0.0185 (BeO). ..
phosphate Be3(PO4)2.6H20 2% CHaCOOH 0.055
10% « 0.1725
BERYLLIUM HYDROXIDE Be(OH)2.
SOLUBILITY IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE.
(Rubenbauer — Z. anorg. Chem. 30 334, '02.)
Moist Be(OH)2 used, solutions shaken 5 hours, temperature prob-
ably about 20°.
Per 20 absolution. Dilution Gms. per 100 cc. Solution.
Gms. Na. Gms. Be. jd^jg NaOH. Be(OH)2."
0-3358 0.0358 1.37 2.917 0.850
0.6716 0.0882 0.68 5-840 2.094
0.8725 0.1175 0.53 7.585 2.789
1.7346 0.2847 0.27 18.310 6.760
SOLUBILITY IN AQUEOUS SODIUM HYDROXIDE AT DIFFERENT TEMPERATURES.
(Haber and Oordt, 1904.)
Normality of Gm. BeO per Liter Sat. Sol, at:
Aq. NaOH.
0-5
I
2
BERYLLIUM OXALATE BeC2O4.3H2O.
100 gms. water dissolve 63.2 gms. BeC2O4.3H2O at 25° (Wirth, 1914.)
o.i n oxalic acid " 75-92 "
o.insulfuric " " 72.65 "
i.on " " 52.8 "
BERYLLIUM PALMITATE and Salts of Other Fatty Acids.
SOLUBILITIES IN ETHYL AND METHYL ALCOHOLS AT 25°. (jacobson and Holmes, 1916.)
Gms. of Each Salt (Determined Separately) per 100 Gms. Solvent.
Solvent. / * • N
Be Palmitate. Be Stearate. Be Laurate. Be Myristate.
Ethyl Alcohol o . 004 ... o . 004 o . 004
Methyl Alcohol o . 042 o . 040 o . 050 o . 047
20-23°.
0.060
50-53°.
0.080
100°.
0.080
0.170
0.570
0.230
0.900
0.290
1.020
Mols. H2O
«. o per i Mol.
* ' BeS04.
SOLUBILITY IN
Gms. BeSO4 per
100 Gms. S<
WATER. (Levi, Malv
m Mols. H20
base. t<». P^e's^01
ano, 1906.)
Gms. BeSO4 per
too Gms.
Solid
Phase.
Water.
Solution.
Water.
Solution.
31
ii. 18
52-23
34-
32 BeS04.6H,0 95.4
6.44
90.
63
47-
55 BeS04.4HO
5°
9.62
60.67
37
77
107.2
5-o6
3
53-
58
"
72.2
7-79
74-94
42
8$
' ill
4-55
14*
•3
56
I9
11
77-4
81.87
45-
01
' 80
6.89
84
76
45
87 B
eSO4 .aH,0
30
13.33
43.78
3°'
45 BeSO
•4lIjO 91.4
5-97
97-
77
49
.42
"
40
12.49
46.74
31-
85
' IO5
4-93
118
4
54
21
"
68
9.42
61.95
38.
27 119
3,91
149.
3
59-88
<4
85
7-65
76,30
43.
28 «
149 BERYLLIUM SULFATE
SOLUBILITY OF BERYLLIUM SULFATE IN AQUEOUS SULFURIC ACID AT 25°.
(Wirth, 1912-13.)
Cms. H2SO< Cms. BeSO« Cms. H2SO4 Cms. BeSCh
per 100 Cms. per 100 Cms. Solid Phase. per 100 Cms. per 100 Cms. Solid Phase.
Solvent. Sat. Sol. Solvent. Sat. Sol.
o 8.212 BeSO4.6H2Q 45.51 6.628 BeSO4.6H2O
5.23 8.429 50-63 5-438 BeSO4.4H2O
9-61 7-944 56.59 3-640
18.70 6.603 63.24 2.244
34 5-63i 65.24 2.128
40.35 5-773 73-64 2.185
Freezing-point data for mixtures of beryllium sulfate and potassium sulfate are
given by Grahmann (i9I3)«
BERYLLIUM MetaVANADATE Be(VO3)24H2O.
100 gms. H2O dissolve o.i gm. of the salt at 25°. (Brinton, 1916.)
BETAINE (Trimethyl glycocoll) C5HUO2N.H2O.
SOLUBILITY OF ANHYDROUS BETAINE IN WATER AND ALCOHOLS.
(Stoltzenberg, 1914-)
(Figures read from the author's curves.)
'• Gms. CsHuCfeN per 100 Gms. Gms. CsHnQiN per 100 Gms.
c2H5OH. HO CKOH. c2H5OH;
-10 134 38 5 5o 197 70 16
o 140 43 6 60 215 75 18.5
+ io 147 49 7 70 236 80 22
20 157 54 8.5 80 259 25
30 168 60 ii 90 286 ..
40 182 65 13 100 328
BETAINE SALTS.
SOLUBILITY OF EACH, SEPARATELY, IN WATER.
(Stoltzenberg, 1914.)
Grams per 100 Grams H2O.
— 10
o
+ 10
20
30
40
50
60
70
80
90
100 169 206
Data are also given by Stoltzenberg for the following basic salts of betaine
(C6HUO2N)2HC1.H2O, (C5HuO2N)2.HBr, (C6HnO2N)2HI, (C6HUO2N)2H2SO4 and
(C6H11O2N)2HAuCl4.H2O.
CsHiiOjjN. CsHnCfeN. CsHnCfeN. CsHnCfcN. CsHnQzN.
CsHnOaN.
CsHnCfcN^
HC1.
HBr.
HI.
H2SO4.H2O.
HsPO4.
HMnO4.
HAuCl4.
38
28
35
67
35
1.5
1.3
44
39
66
86
45
i-75
1-5
52
S2
98
107
58
2-5
2
60
65
130
132
73
5
3
70
79
162
164
91
9
4.5
8l
94
198
203
112
16
6
93
no
231
250
135
30
8
106
127
269
306
160
(55°) 48
n-5
120
144
304
. . .
190
15
135
162
(75°) 321
. . .
223
18
!5X
183
23
BETOL 03-Naphthylsalicylate)
Freezing-point data'including super solubility curves, are given for mixtures of
betol a-nd salol by Miers and Isaac, 1907.
BISMUTH 150
BISMUTH Bi.
RECIPROCAL SOLUBILITIES, DETERMINED BY THE METHOD OF LOWERING OF
TUSION-POINT (see footnote, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
Bismuth + Bromine (Eggink, 1908.)
" 4" Chlorine "
+ Iodine (Amadori and Becarelli, 1912.)
" + Sulfur (Aten, 1905; Palabon, 1904.)
MUTUAL SOLUBILITY OF BISMUTH AND ZINC. (Spring and Romanoff, 1906.)
t °.
266
419
475
Upper Layer.
Lower^ Layer.
t °.
584
650
75o
Upper Layei .
Lower Layer.
°86
84
%Zn.
14
16
3
5
%Zn.
97
95
80
77
70
%Zn.
20
23
30
10
15
27
90
85
73
810-820 (crit. temp.)
BISMUTH CHLORIDE. BiCl3. BSMUTH OxyCHLORIDE BJOC1.H2O.
SOLUBILITY IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID.
Results at 25°. (Noyes and Hall, 1917.) Results at 30°. (Jacobs, 1917.)
Cl.
Bi. H( = Cl-3Bi).
Bi2O3. HC1.
1.002 0.3477
0.00130 0.3438
0.60 2.40 BiOCl.HaO
1.007 0.4350
0.00376 0.4237
5-35 5-69
i. oio 0.5221
o . 00869 o . 4960
8.17 8.47
I.OI3 0.6244
0.01767 0.5714
8.70 8.93
.018 0.7375
0.03138 0.6434
14.52 13.02
.025 0.8824
0.05338 0.7223
18.60 15.80
.036 1.0760
0.08937 0.8079
30.10 21.7
.044 1.2277
O.II77 0.8746
36.95 25.4
.061 1.5321
O.lSlO 0.9891
54.70 31-5
.083 1.9021
0.2657 I.I05
56 32.8 BiOCl
.157 3-1865
0.5685 1.481
58.5 33 BiCl^H^
.237 4.5056
0.9022 1-799
56.6 33.8 +BiCU
.288 5.325
i. 100 2.025
56.25 34.9 BiCU
.329 6.066
1.317 2.115
55-9 35-9 BICU.HCI
SOLUBILITY
OF BISMUTH CHLORIDE
IN SEVERAL SOLVENTS.
Cms. I
5iCb per 100.
to
. . A ., -
solvent.
cc. Solvent.
Cms. Solvent. Authority.
Acetone
18° ... 17.
9 (^is=O.9I94)(Naumann, 1904/05.)
Ethyl Acetate
18° ... i .
66 (Ji8 = O.9Io6)(Naumann, 1910).
Anhydrous Hydrazine ord. temp. 32 ... (Welsh and Broderson, 1915.)
loo gms. 95% formic acid dissolve 0.05 gm. bismuth oxychloride (BiOCl) at
19.8°. (Aschan, 1913.)
Freezing-point data are given for BiCl3+CuCl, BiCl3+FeCl3, BiCl3-f PbG2,
BiCl3-f-PbBr2 and BiCl3+ZnCl2 by Herrmann (1911) and for BiCl3+TlCl by
Scarpa (1912).
BISMUTH CITRATE (CH2)2C(OH)(COO)3Bi. BISMUTH Ammonium
CITRATE.
SOLUBILITY OF EACH IN WATER AND IN AQUEOUS ETHYL ALCOHOL AT 25°. (Seidell. '10.)
-«*4
o o.on o 22.25 1.25
51 0.041 51 1.34 0.92
91.4 0.065 91.4 None 0.81
151 BISMUTH HYDROXIDE
BISMUTH HYDROXIDE Bi(OH),.
SOLUBILITY OF BISMUTH HYDROXIDE IN AQUEOUS SOLUTIONS OF SODIUM
AND POTASSIUM HYDROXIDES AT 20° AND AT 100°.
(Moser, 1909.)
Cms KOH Gms> Dissolved Bi(QH)3 per Liter at: Qmg j^aOH ^ms. Dissolved Bi(OH)j per Liter at:
per Liter. ' ^~ — ^T * perLiter. ' 20^ I0o». *
28 o 0.188 20 o 0.188
50 trace 0.249 4° trace (0.0014)* 0.249
112 0.037 °-373 80 0.050 (0.0029)* 0.436
168 0.074 ... 120 0.087(0.0054)* 0.622
224 o.ioo 0.622 160 o.ioo ...
280 0.124 0.622 200 0.124 , 0.622
336 0.137 ... 240 0.137
448 0.137 1.494 320 0.137 1.494
560 0.174 2.054 400 0.199 2.120
* Results at 25° by Knox (1909).
At 100° some Bi(OH)3 was converted into BiO(OH).
SOLUBILITY OF BISMUTH HYDROXIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AND OF POTASSIUM BROMIDE AT 30°.
(Herz and Bulla, 1909.)
(An excess of bismuth hydroxide, prepared according to Moses and having the
composition corresponding to BiO.OH, was shaken 2-3 weeks at 30° with aqueous
KC1 and KBr. The analyses of the sat. solutions are expressed in terms of milli-
mols KOH and KC1 or KBr. They have been calculated for the following
table to gms. BiO.OH and KC1 or KBr.)
Gms. per 100 cc. Sat. Sol. Gms. per 100 cc. Sat. Sol.
' - '
SolVCnt- BiO.OH. KCl ' BiO.OH. r
2nKC\ 3.759 13.75 iwKBr 8.555 7.67
3^KC1 5-745 20.71 2wKBr 17.785 15.02
BISMUTH IODIDE BiI3.
100 gms. absolute alcohol dissolve 3.5 gms. BiI3 at 20°. (Gott and Muir, 1888.)
• 100 gms. methylene iodide, CH2l2, dissolve 0.15 gm. BiI3 at 12°. (Retgers, 1893.)
BISMUTH NITRATE Bi(NO3)3.5H2O.
100 gms. acetone dissolve 48.66 gms. Bi(NO3)3.5H2O at o°, and 41.7 gms. at
IQ « (von Laszczynski, 1894.)
SOLUBILITY OF BISMUTH NITRATE IN AQUEOUS NITRIC ACID AND IN AQUEOUS
NITRIC ACID CONTAINING ACETONE, AT ORDINARY TEMPERATURE.
(Dubrissay, 1911.)
SolidPhaSC-
0.922 n HNO3 86.86 Bi(N03)3.5H2O
0.922" " + 6.66% Acetone 85.51
0.922" " +13.33% " 81.96
2.3 " " 80.37
2.3 " " +16.66% 74.47
SOLUBILITY OF DOUBLE NITRATES OF BISMUTH AND MAGNESIUM, NICKEL,
COBALT, ZINC AND MANGANESE IN CONC. HNO3 AT 16°.
(Jantsch, 1912.)
(di6 of HNO3 = 1.325, ioo cc. of this acid contained 51.59 gms. HNOa.)
Gms. Hydrated Gms. Hydrated
Double Salt. Salt per ioo cc. Double Salt. Salt per ioo cc.
Sat. Solution. Sat. Solution.
Bi2Mg3(NO3)i2.24H2O 41 -69 Bi2Zn3(NO3)i2.24H2O 57 .51
Bi2Ni3(NO3)12.24H2O 46.20 Bi2Mn3(N03)i2.24H2O 65.77
Bi2Co3(NO3)i2.24H2O 54 . 67
BISMUTH OXIDE
152
BISMUTH OXIDE Bi2O3.
SOLUBILITY OF BISMUTH OXIDE IN AQUEOUS NITRIC ACID AT 20°.
(Rutten and van Bemmelen, 1902.)
Present in Shaker
Flask.
Gms. per TOO Gms.
Solution.
Mols. per 100 Mols. H2O.
Solid
Per i part Bi2Os.
3N2O5.ioH2O.
Bi203
N20S
Bi203
N206 R
fSfof3
Phase.
24.4 parts H-P
3.2 parts H2O
0.321
6.37
0.963
7.17
o 126
2.844
1.61
13.82
i
12.8)
4.8 (
B52O3.N2O6.2H2O
Dilute HNO3
Dilute HNO3
18.74
31.48
15-9
23-7
10.50
27.2
38.65
83.8
i
i
3-6}
3.Q J
Bi2OsN205.H20
Dilute HNO3 =
6.13% N2OS
32-93
24.83
3°-I5
97-97
»
Bi2O,.N2O5.HjO and
Bi203.3N205.ioH20
6.816% N205
32.67
24.70
29.70
96.57
i
3-21
24.0% N2O6
51.0% N206
24.16
11.66
28.25 ...»
46.62
19.65
10.81
98.76
186.23
i
i-
5-0
17.2 J
Bi2O3.3N2Os.ioH2O
70.0% N206
20.76
53-75
33-51
355.87
i
io.6j
27.85
51.02
51.0
403.0
i
7-9 {
Bi2O3.3N2O5.ioH2O and
Bi203.3N205.3H20
Anyhdrous HNO
Bi203+ "
38.56
4-05
68.28
74.90
14-35
7-45
492.0
592.9
j
34-31
79-5*
Bi208.3N,06.3HaO
Results are also given for 9°, 30°, and 65°.
BISMUTH TriPHENYL Bi(C6H6)3.
Fusion-point data (see footnote, p. i) are given for mixtures of bismuth
triphenyl and mercury diphenyl by Cambi (1912).
BISMUTH SALICYLATE (basic, 64% Bi2O3).
SOLUBILITY IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Gms. C2HsOH per
100 Gms. Solvent.
Gms. Salt per
100 Gms. Sat. Sol.
Gms C2H6OHper
zoo Gms. Solvent.
Gms. Salt per
100 Gms. Sat. Sol.
O
O.OIO
80
0.065
20
0.015
00
0.095
40
60
0.022
0.036
92.3
100
O.IO5
0.160
BISMUTH SELENIDE Bi2Se3.
Fusion-point data (see footnote, p. i) are given for mixtures of bismuth sele-
nide and silver selenide by Pelabon (1908).
BISMUTH SULFIDE Bi2S3.
i liter H2O dissolves 0.00018 gm. Bi2S3 at 18°.
(Weigel, 1906; see also Bruner and Zawadski, 1912.)
SOLUBILITY OF BISMUTH SULFIDE IN AQUEOUS ALKALI SULFIDE SOLUTIONS AT 25°.
(Knox, 1909 )
Gms. Bi2Ss per
Solvent. 100 cc. Sat. Solvent.
Solution.
0.5 n Na2S
wNaOH
0.0040 0.5
i.on " 0.0238 i
1.5 n " 0.1023 0.5
o.5«K2S 0.0043 I
i n ' 0.0337 1.25 n K2S +i.25wKOH
1.5 w " 0.0639
Freezing-point data (see footnote, p. i) are given for mixtures of bismuth
sulfide and bismuth telluride by Amadori (1915).
Gms. BizSs per
loo cc. Sat.
Solution.
0.0185
0.0838
o . 0240
0.1230
0.2354
BORAX, see sodium tetraborate, p. 629.
I53 BORIC ACID
BORIC ACID H3B03.
SOLUBILITY OF BORIC ACID IN WATER.
(Nasini and Ageno, 1909.)
. 0 Gms. HsBOa per
1 • loo Gms. Sat. Sol.
,0 Gms. HsBOs per
100 Gms. Sat. Sol.
to Gms. HaBO3 per
100 Gms. Sat. Sol.
— o.76Eutec
2.27
30
6.30
80
19.11
0
2-59
40
8.02
90
23.30
+ 10
3-45
50
10.35
100
28.7
20
4.8
60
12.90
1 10
38-7
25
5-5
70
15.70
120
52.4
The results of Herz and Knoch (1904), and one determination by Auerbach
(1903), given in terms of gms. per 100 cc. sat. solution, appear to be in good
agreement with the above. The earlier data of Ditte (1877) are low.
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF HYDROCHLORIC,
SULPHURIC, AND NITRIC ACIDS AT 26°.
(Herz — Z. anorg. Chem. 33, 355. 34. 205, '03.)
Normality of Normality of Gms. Strong Acid Gms. B(OH)3 per 100 cc. Solution,
the H2SO4, HC1 Dissolved per 100 cc
or HNO3. B(OH)3. Solution. In HC1. In H2SO4. In HNO3.
o 0.91 o 5.64 5.64 5.64
0.5 0.78 5 4.0 4.25 4.50
i.o 0.71 10 3-2 3.6 3.9
2.0 0.58 15 2.45 3-o 3-35
3.0 0.49 20 1.8 2.5 2.9
4.0 0.41 25 2.0 2-55
5-o 0-35 30 ••• i-55 2.1
6.0 0.26 35 ... ... 1.75
The determinations given in the original tables in terms of normal
solutions when plotted together lay close to an average curve drawn
through them. The figures in the tables here shown were read (and
calculated) from the average curve.
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF ELECTROLYTES
AT 25°.
(Bogdan — Ann. Scient. Univ. Jassy, 2, 47, 'oz-'o3.)
Gms. Electro-
Grams H3BO3
per
too Gms.
H2Oin
Aq. Solutions of:
Gms. H2O.
NaCl.
KC1.
NaNO3.
KN03.
Na2S04.
K2SO-4.
O
5
•75
5
•75
5
•75
5-75
c
•75
5-75
IO
5
•75
r
.80
5
.78
5.8l
5
.88
5-92
20
5
•74
5
.86
5
.81
5.88
6
• oo
6.10
40
5
.72
3
.98
5
.87
6.04
6
•33
6.50
60
5
.72
6
.12
5
•95
6. 20
6
.70
6.92
80
5
•7i
6
.29
6
.02
6.37
7
.10
7-40
Interpolated from the original.
BORIC ACID 154
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID
AND OF ALKALI CHLORIDES AT 25°. (Herz, 1910.)
(The original results are given in millimols per 10 cc. They have been calcu-
lated to gram quantities, plotted on cross-section paper and the following values
read from the curves.)
Cms. HC1 or Alkali Cms. HsBOs Dissolved per 100 cc. Sat Sol. in Aq.:
Chloride per 100 cc.
Sat. Sol.
O
2
4
6
8
10
15
20
30 ... 6.55
THE SYSTEM BORIC ACID, ACETIC ACID AND WATER AT 30°. (Dukelski, 1909.)
(The sat. solutions _and residues were analyzed by titrating total acidity with
o.i n NaOH and the acetic acid alone by an iodometric method.)
HCl.
Lid.
NaCl.
RbCl.
KCl.
5-59
5-59
5-59
5-59
5-59
4.92
5-20
5-4o
5.60
5-67
4-36
4.85
5-30
5-62
5-75
3.88
4-45
5.20
5-67
5.85
3-50
4.07
5-i5
5-72
5-9°
3-i5
3-75
5.10
5-77
6
3
5-07
5-90
6.25
6.10
6.50
Cms. per 100 Gms.
Sat. Sol.
Solid
Phase.
B(OH)3
Gms. per 100 Gms.
Sat. Sol. Solid
Gms. per 100 Gms.
Sat. Sol. Soiid phase.
BiOs. (CH3CO)20.
3-55
3-i8 7.78
2.98 16.44
2.34 28.96
1.98 41.06
i-47 52-63
1. 12 67.76
B203. (CH3CO)2O.
I.OI 73.96 B(OH)3
0-54 80.67
0.45 84.55 "+(?)
0.39 84.65
O.4I 84.48
o . 46 84 . 44
0.50 84.51
B203. (CH3CO)20.
4.98 82.13 B203.2(CH3CO)20
5.13 84.60
5.41 85.68
4.82 88.74 BzOs.sCCHsCO)^
4.71 89.98
4.06 92.68
3.10 95.76
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF:
Acetic Acid at 26°. (Herz, 19030.) Acetone at 2O°. (Herz and Knoch, 1904.)
Normality of Solutions. Gms. per 100 cc. Solution. cc> Acetone B(OH)3 per 100 cc. Solution.
CHaCQOH. B(OH)'3. CHaCOOH. B(OH)3. ^SoiwnU* Millimols. Grams!
0 0-91 o 5-64
1 0.82 5 4.7
2 0.65 1C 4-2
4 0.42 20 3.0
6 p. 25 30 2.0
o
79 -J5
4.91
20
81.71
5-o7
30
83-35
5-*7
40
82.72
5-*3
50
81.62
5-06
60
76.40
4-74
70
67.62
4.19
80
55-05
3-4i
100
8.06
0.50
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF UREA, ACETONE,
AND OF PROPYL ALCOHOL AT 25° (Bogdan.)
Grams of Gms. HaBOs per 100 g. H2O in Aq.
CO(NH2)2,(CH3)2CO Solutions of:
or of CsHyOH per
100 Gms. H2O.
O
10
20
40
60
CO(NH2)2
(CH3)2CO.
CaHyOH.
5-75
5-75
5-75
5-84
5-84
5.80
5-93
5-93
5-85
6.13
6.12
5-94
6.31
6.29
6.03
155
BORIC ACID
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF SEVERAL ALCOHOLS AT 25°.
(Mueller and Abegg, 1906.)
In Aq. Methyl Alcohol. In Aq. Ethyl Alcohol.
In Aq. Propyl Alcohol.
Solvent.
Gms. HaBOa Solyent. Gms. HaBOa Solvent.
</ of Gms.HaBOj
dv
Wt.
CHaO
% per 100 cc.
H. Sat. Sol. 4y
Wt. %
C2HsOH.
per loo cc.
Sat. Sol. <**f •
cM.
_ T per too cc.
Sat. Sol. sat gol.
0.9691
19
5
•55
0.9714
20.2
5-14
0.9043
50.83
O
9193
3 99
0.9340
41-
5 6
•27
0.9350
42.3
4.96
0.8231
79-41
o
.8570
2.83
0.9185
50
6
.81
0.8789
67'- 3
4.52
0.8133
95-5
o
.8466
3.58
0.9019
58
7
.20
0.8576
76.2
4-34
0.8010
IOO
o
.8297
5-96
0.8842
66
8
. 10
0.8198
91.1
5-54
0.7960
IOO
17
-99*
0.8089
95
6.85
*
J
0.7947
IOO
9-47t
+ A — « flf ft
d*t =
0.8904.
j "-25 — W«UDO»J»
In Aq. i Butyl Alcohol.
Solvent. j _f Gms. HaBOa
In Aq. i Amyl Alcohol.
v
Mol. %
CJfcOH.
Sat. Sol.
per loo cc.
Sat. Sol.
0.9923
0.70
1.0124
5.48
0.9853
2.15
1.0038
5-32
0.9855
2.18
1.0046
5-32
0.8173
71-4
0-8351
2
0.8133
77.1
0.8220
2-15
0.8081
85-6
0.8195
2.6l
0.7984
IOO
0.8172
4-30
Solvent.
Mol. %
•y*
CsHuOH.
0.9943
0.448
0.9936
0.520
0.9931
0.525*
0.8232
67.26f
0.8183
75-54
0.8142
83.40
0.8068
IOO
d of Gms.HaBOs
Sat. Sol. ^tVsa?
1.0132
1.0125
1.0123
0.8290
0.8253
0.8223
0.8220
= HzO sat. with amyl alcohol.
t = Amyl alcohol sat. with H2O.
5.48
5.46
5.46
I. 60
1.69
1.98
3.54
One liter H2O saturated with amyl alcohol dissolves 55.5 gms. H3BO3 at 15°.
(Auerbach, 1903.)
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF ETHYL
ALCOHOL AT 15° AND AT 25°.
(Seidell, 1908.)
Results at 15°. Results at 25°.
disof
Sat. Sol.
Gms. C2H6OH Gms.HaBOs
per loo Gms. per 100 Gms.
Solvent. Sat. Sol.
1.014
O 4. II
0.9986
8.9 3.90
0.9658
32 3.58
0.9268
51 3-48
0.8820
70.2 3.22
0.8389
91.3 5.06
0.8370
93-6 5-70
0.8356
99.8 9.18
(*250f
Sat. Sol.
Gms. C2H»OH
per loo Gms.
Solvent.
Gms. per 100 Gms. Sat. Sol.
' HaBOa.
CzHsOH.
1.018
O
5-42
O
0-987
20
5-20
18.96
0.952
40
5-io
37-96
0.908
60
5
57
0.862
80
5-05
75.96
0.853
85
5-30
80.50
0.842
90 ,
6.20
84.4
0.838
95
8
87.4
0.838
IOO
ii. 20
88.8
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF LACTIC ACID,
OXALIC ACID, d and i TARTARIC ACIDS AT 25°.
In Aq. Lactic Acid.
(Mueller and Abegg, 1906.)
In Aq. Oxalic Acid.
(Herz, 1910.)
In Aq. d and i Tartaric Acid.
(Herz, 1911.)
Solvent.
d Mol. %
V CaHeOa.
d of Gms. HaBO
c To i Per I0° cc-
Sat. Sol. sat. Sol.
a Gms. per 100 cc.
Sat. Sol.
Solid Phase.
Gms. per 100 cc.
Sat. Sol.
H2C204.
HaBOa
C4H606.
HaBOa.
1.0252
2
.321
1.0444
6
•64
2.26
6.17
HaBOa
O
5-59
1.0722
6
.819
1.0986
9
.98
5.36
6.70
"
11.25
JAcid
6.20
1.1405
18
-77
1-1635
II
•53
12.39
7-44
" +H2C20«
22.5
"
6.63
I . 2023
36
•33
1.2254
12
.90
11.27
3-45
H2C204
45
M
7.48
10.84
0.97
"
9-45
i Acid
6. ii
10.77
0-55
"
18.90
M
6.48
10.63
0
"
37
"
7-23
BORIC ACID
156
SOLUBILITY OP BORIC ACID IN:
Pure Glycerol (Sp.Gr. =1.260
at 15.5°)-
iHooper — Pharm. J. Trans. [3] 13, 258, '82.)
Aq. Solutions of Glycerol
at 25°.
(Herz and Knoch — Z. anorg. Chem. 45, 268, '05.)
Cms. B2O3
t o 3H2O per
100 CC.
Glycerine
•"' Cms. B(OH)3 per 100
Gms.
Wt. % Millimols
Glycerine B(OH)3 per
in Solvent. 100 cc. Sol.
Sp. Gr.
t 25°
Gms. B(OH)3
per TOO
Glycerine. Solution.
av
cc. Solution
Gms .So-
lution.
0
20
15
.87
I3-1?
O
90.1
.017
5
•59
5-50
10
24
J9
.04
16.00
7
•J5
90.1
.038
5
•59
5-38
20
28
22
.22
.18.21
20
•44
90.6
.063
5
.62
5.28
30
33
26
.19
20.75
3i
•55
92.9
.090
5
.76
5'29
40
38
30
.16
23-I7
40
•95
97-0
•"3
6. 02
5-41
50
44
34
.92
25-95
48
•7
103.0
•J33
6
•39
5-64
60
So
39
.68
28.41
69
.2
140.2
.187
8
.69
7-32
70
56
44
•65
30.72
100
• O
300.3 1.272
24
.20
19.02
80
61
48
.41
32.61
90
67
53
.18
34-70
100
72
57
.14
36-36
IN AQUEOUS SOLUTIONS OF GLYCEROL
AT 25°.
(Mueller and Abegg, 1906.)
Solvent.
I.IS74
Mol. % Wt. %
3sH(
60
j of Gms. HsBOs
TC- per ioo cc.
Sat. Sol. Sat. Sol.
AQUEOUS SOLUTIONS OF DULCITE
AT 25°.
(Mueller and Abegg, 1906.)
Solvent.
24.64
46.75
1.2370 67.71
1.2531 90.58
ioo gms. glycerol
, Mol. %
dV C6H8(OH)6.
0.9995 0.065
I.OOlS 0.130
I. 0060 0.260
Of Gms. HsBOa
' , per ioo cc.
Sol. Sat. Sol.
I. 0686 5.50
I. 0212 5.63
1.0260 5.81
1.1707 7.49
1.2260 13.22
90 1.2526 18.35
96.6 1.2710 23.44
1.256) dissolve n gms. H3BO3 at i5°-i6°.
(Ossendowski, 1907.)
ioo gms. dichlorethylene dissolve 0.006 gm. H3BO3 at 15°. (Wester and Brunis, 1914.)
ioo gms. trichlorethylene dissolve 0.016 gm. H3BO3 at 15°. " "
ioo cc. anhydrous hydrazine dissolve 55 gms. H3BO3 at room temp.
(Welsh and Broderson, 1915.)
SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF MANNITE AT 25°
AND VICE VERSA.
(Ageno and Valla, 1912, 1913.)
Grams per ioo cc. Sat. Sol.
Solid Phase.
HsBOj.
CsHwOe.
5-50
0
H3BO3
5-90
1.82
"
6.29
5.46
"
6.44
7-28
tt
6.64
9.II
"
6.83.
10.93
"
7.08
12-75
tt
7.27
14.57
tt
7.71
18.99
tt
HsBOs.
C6Hl406.
OUIIU K lldoC.
8.70
25.65
H3B03
9-43
32.43
" +C6H1406
7.71
27-97
C6H1406
5-75
25.65
, - '
4.92
24.65
u
3-46
23-03
tt
2.87
22.98
tt
1.64
20.80
"
0
19.58
tt
Additional determinations at 30° also given.
Determinations at 25°, differing somewhat from the above, are given by Mueller
and Abegg (1906). * -
Data for the system boric acid, phenol and water are given by Timmermans
(1907).
157
BORIC ACID
DISTRIBUTION OF BORIC ACID BETWEEN WATER AND AMYL ALCOHOL
AT 25°.
(Fox — Z. anorg. Chem. 35* 130, '03.)
Millimols B(OH)3 in Cms. B(OH)3 in 100 cc.
Aq
Alcoholic
Aq.
Alcoholic
Layer.
Layer.
Layer.
Layer.
26S
.8
76
.6
I
.648
0
•475
196
•5
59
•5
I
.219
0
•369
159
.6
47
•5
O
.990
O
.294
126
.0
37
,i
O
.781
O
.230
Millimols B(OH)3 in
Cms. B(OH)3 in 100 cc
TAq.
Layer.
87.9
75-2
64.6
Alcoholic
Layer.
33-2
22 .7
19.76
Aq.
Layer.
0-545
0.466
0.400
Alcoholic
Layer.
O.2O6
O.I4I
0.123
RESULTS AT 15°. (Mueller and Abegg, 1906.)
Millimols B(OH)3 per Liter. Gms. B(OH)3 per 100 cc. Mifflmok.BCOH), per Gms. B(OH)3 per 100
Aq. Layer.
Alcohol
Layer.
Aq.
Layer.
Alcohol
Layer
Aq. Layer.
Alcohol
Layer.
Aq.
Layer.
Alcohol
Layer.
894
264
5
-44
I .64
427.4
127.6
2
•65
0.79
607.2
176.4
3
.76
1.09
372
1 10
2
.31
0.68
589-3
177-4
3
-65
I .IO
289.1
84.9
I
'79
0-53
Data agreeing with those of Fox at 25° are afso given by Mueller and Abegg,
1906. One determination at 35° gave 0.907 gm. B(OH)3 per 100 cc. aq. layer and
0.274 gm. per 100 cc. alcohol layer.
DISTRIBUTION OF BORIC ACID BETWEEN AQUEOUS SODIUM CHLORIDE
SOLUTIONS AND AMYL ALCOHOL AT 25°.
(Mueller and Abegg, 1906 )
Gms. per 100 cc.:
Aq. Layer. Alcohol Layer.
NaCl.
O
5-53
8.72
10.91
13-84
HsBOs. H20.
5-46 7 39
6.40
5-90
5-46
5-15
5-37
5-27
5-23
5-i6
•65
•65
.67
.69
•77
Alcohol
Layer.
0.8296
0.8277
0.8268
0.8259
0.8254
Gms. per
Aq. Layer.
100 cc.:
Alcohol Layer.
NaCl.
H3B03.
H20. HsBOs.
16.64
5-13
4.71
•79
17.90
5.02
4-31
•79
20.36
5-02
4.19
.87
23-52
4-97
3-59
.96
25-03
4-95
3-20
•99
d^ of
Alcohol
Layer.
0.8247
O . 8241
0.8240
0.8233
0.8229
DISTRIBUTION OF BORIC ACID BETWEEN WATER AND MIXTURES OF AMYL
ALCOHOL AND CARBON DISULFIDE AT 25°.
(Herz and Kurzer, 1910.)
50 Vol. %C6HUOH+50
Vol. % CSa.
Gms. HaBOs per 100 cc.
Aqueous
Layer.
0.469
0.839
I .207
75 Vol. %C.HnOH+25
Vol. % CS,.
Gms. HsBOs per 100 ec.
25 Vol. %C5HnOH+95
Vol. % CSa.
Gms. HsBOs per 100 cc.
Aqueous
Layer.
0.387
0-743
I.I43
1.590
CoHuOH+CSa.
Layer.
0.095
O.I7I
0.266
0-365
C5HiiOH+CS2.
Layer.
Aqueous
1.791
0.095
0.161
0.226
0-344
'Yqut
Layer.
0-433
0.910
1-343
1.940
CsHuOH+CSz.'
Layer.
0.053
0.108
0.164
0.238
BORIC ANHYDRIDE B2O3.
Fusion-point data (solubilities, see footnote, p. i) are given for mixtures of
B2O3+CaO and B2O3+SrO by Guertler (1904).
BORIC ACID (Tetra) H2B4O7.
TOO grams water dissolve 2.69 grams H2B4O/ at 15°, Sp. Gr. = 1.015.
(Gerlach, 1889.)
BORON TRI-FLUORIDE BF3.
i cc. H2O absorbs 1.057 cc> BF3 at o° and 762 mm.; i cc. cone. H2SO4 (Sp. Gr.
1.85) absorbs 50 cc. BF3.
BRASSIDIC ACID 158
BRASSIDIC ACID
Solubility data determined by the freezing-point method are given by Mas-
carelli and Sanna (1915), for mixtures of brassidic and erucic acids and brassidic
and isoerucic acids.
BROMAL HYDRATE CBr3.CH(OH)2
The distribution coefficient of bromal hydrate between olive oil and water is
0.665 at ord. temp. (Baum, 1899); 0.7 at ord. temp. (Meyer, 1909).
BROMINE Br.
SOLUBILITY IN WATER.
fWinkler — Chem. Ztg. 23, 687, '99; Roozeboom — Rec. trav. chim. 3, 29, 59, 73, 84, '84; Dancer —
J. Chem. Soc. 15, 477, '62; at 15°, Dietze — Pharm. Ztg. 43, 290, '08 J
Grams Bromine per 100 Grams. __^
Solubility."*
* * Water. Solution.
(W.) (R. D. & D.) (W.) (R. D. & D.) ff-
o 4-^7 4.22 3-98 4-05 60.5 43.1
5 3-92 3-7 3-77 3-57 45-8 32-4
10 3.74 3-4 3-61 3-29 35-1 24.8
15 3-65 3-25 3-S2 3-J5 27.0 19.0
20 3.58 3.20 3.46 3.10 21.3 14.8
25 3-48 3-J7 3-36 3-o7 17 o 11.7
30 3.44 3-!3 3-32 .3-03 13-8 9-4
40 3.45 ••• 3-33 ••• 9-4 6.2
50 3.52 ... 3.40 ... 6.5 4.0
60 ... 4-9 2.8
80 ... ... 3-o LI
* For definition of "Absorption Coefficient " a and "Solubility '' q, see Acetylene, p. 16.
One liter sat. solution of bromine in water contains 0.21 mol. Br2 = 33.56
gms. Br at 25°. (Bray and Connolly, 1910.)
The coefficient of solubility of bromine in water at 15°, determined by an
aspiration method, is given as 33 by Jones (1911). This investigator also gives
the figure 56 for the solubility coefficient in 25 vol. % acetic acid and 551 for
90 vol. % acetic acid at 15°.
Data for the distribution of bromine between water and air at 25°, are given
by Hantzsch and Vagt (1901).
SOLUBILITY OF BROMINE IN AQUEOUS SOLUTIONS OF MERCURIC BROMIDE
AT 25° AND VICE VERSA.
(Herz and Paul, 1914.)
Gms. per 100 cc. Sat. Sol. Soiy Gms. per 100 cc. Sat. Sol. Solid
HgBrz. Br. Phase. HgBr2. fiT Phase.
o 3.40 Br2 0.763 3.57 Br2+HgBr2
0.202 3.53 0.701 2.88 HgBr2
0-285 3-55 0.664 1-20
0.462 3.56 "
159
BROMINE
SOLUBILITY OF BROMINE IN AQUEOUS SOLUTIONS OF POTASSIUM BROMIDE.
(Results at o° and 25°, Boericke, 1905; at o°, Jones and Hartmann, 1916;
at 18.5° and 26.5°, Worley, 1905.)
Cms. Bromine Dissolved per Liter of Sat. Solution at:
Br per Liter.
Liter.
o°.
18.5°.
25°.
26.5°.
0
0
41.6 (24.2)
35-56
34
34-23
O.OO5
o-59
41-7 (25-5)
36.1
34.3
35-i
0.010
1.19
42.6 (26.2)
37
35
36
0.020
2.38
44.4 127.5)
38.56
36.5
37-35
o . 050
5-95
50.2 (31.5)
43-8
4i
42.5
0.100
11.90
59-7 (4o)
52-23
49-3
51.87
O.2O
23.80
79-i (57-i)
69.69
67-3
68.69
0.50
59-5i
138.6 (111.9)
123
119
116
0.80
92.22
200 (174)
178.70
176
168 . 10
I
119.02
243.1 (217.5)
216
216.5
204
I-725
205.2
402.3 (395-9)
. . .
. . .
...
1.82
216.6
423.8 (423)
...
...
•
2.17
258.2
5II.7 (5H.7)
. . .
...
...
3-033
360.8
736.7 ...
632.4
Very accurate determinations at o°, at concentrations of KBr below o.oi
normal, are given by Jones and Hartmann. Liquid bromine in contact with
aqueous solutions at o° is slowly converted to the hydrate, Br2.ioH2O, with a
reduction in amount of dissolved bromine. At this temperature there are, con-
sequently, two saturation concentrations. The unstable one being for solutions
in contact with liquid bromine and the stable one being for solutions in contact
with Br2.ioH2O. The results for the latter are shown in parentheses in the
above table.
SOLUBILITY OF BROMINE IN AQUEOUS SOLUTIONS OF POTASSIUM SUL-
PHATE, SODIUM SULPHATE, AND OF SODIUM NITRATE AT 25°.
(Jakowkin — Z. physik. Chem. 20, 38, '96.)
Normality o:
Salt Solution
i
1
In K2S04
Gms. per Liter.
In Na2SO4
Gms. per Liter.
In NaNOs
Gms. per Liter.
9I.I8
45-59
22.79
5-69
Br.
25.14
29.44
31.46
32.70
33 ^o
Na2SO4.
15.88
7-94
3-97
Br. "
25.07
29.20
32-94
33-26
NaN03.
85.09
42-54
21.27
10.63
5-31
Br.
28.80
31-35
32.62
33-33
33-74
SOLUBILITY OF BROMINE IN AQUEOUS SALT SOLUTIONS AT 25°.
(McLauchlan, 1903.)
Gms.
Normality
Gms.
Gms.
Normality Gms.
Salt.
Salt per
of Dis-
Br. per
Salt. Salt per
of Dis- Br. per
Liter.
solved Br.
Liter.
Liter.
solved Br. Liter.
Water
0.0
0.424
33-95
NH4NO3 80. 1 1
0.688 55.15
Na2S04
63-55
0.286
23-9
I^aCl 58.50
0.701 55.90
K2S04
9I.I8
0.310
24.8
KC1 74.60
0.718 57.40
(NH,)2SO4
70.04
0.971
77-7
NH4C1 53.52
1.028 82.2
NaNO3
VKTr\
85.09
0-3495
28.0
CH3COONH477.o9
4.26 340.5
KNO3
101.19
0.362
28.95
H2SO4* 49-03
0.366 29.26
* Wildeman.
BROMINE
160
SOLUBILITY OF BROMINE IN AQUEOUS SOLUTIONS OF SODIUM BROMIDE AT 25°.
(Bell and Buckley, 1912.)
Grams per Liter Sat. Sol. j^ of
NaBr. Ei. Sat. Sol.
92.6 99.2 I.2I3
160.5 176.7 1.372
205.8 247.8 1-515
255-8 343 1-678
RECIPROCAL SOLUBILITY OF BROMINE AND CHLORINE, BROMINE AND HYDRO-
BROMIC ACID AND BROMINE AND SULFUR DlOXIDE, DETERMINED BY METHOD
OF LOWERING OF THE FREEZING-POINT (see footnote, p. i).
Gms. per Litei
• Sat. Sol.
d>* of
Sat. Sol.
1.997
2.137
2.327
2.420
NaBr.
319-7
359
408 '.3
Br.
546
641 .6
769.2
834
Results for Bromine
+ Chlorine.
(Lebeau, 1906; see also
Karsten, 1907.)
Bromine + Hydro-
bromic Acid.
(Buchner and Karsten, 1908-09.)
Bromine -f- Sulfur
Dioxide.
(van der Goot, 1913.)
t°of
Melting.
Gms. Br per
loo Gms.
Mixture.
" t°of
Melting.
Gms. Br per
loo Gms.
Mixture
Mol. %
Br. in
Mixture.
t°of
Melting.
Gms. Br per
loo Gms.
Mixture.
—
102.5
O
-87-3
0
O
-75-i
0
.—
IOO
6
•5
-90
6
2.
5
-75-3*
I
•73
—
90
31
-95*
II
.2
4-
8
-60
4
—
80
48
.6
-90
II
.8
5
-40
12
-5
—
70
60
-4
-80
15
.2
.6.
8
-30
21
—
60
70
-70
22
n.
5
— 20
35
•5
—
50
79
-60
31
-7
19
-18
40
•5
— •
40
86
•3
— 50
43
30
-16
48
—
30
91
.1
-40
54
•5
43-
5
-14
72
—
20
95
.2
-30
66
.2
60
-13
90
—
IO
89
— 20
79
•5
76.
5
— 10
96
•5
—
7-3
IOO
-12.5
90
90
— 7.1
IOO
* Eutec..
SOLUBILITY DATA, DETERMINED BY THE FREEZING-POINT METHOD (see footnote,
p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
Bromine + Methyl alcohol (Maass and Mclntosh, 1912.)
+ Ethyl alcohol
" + Ethyl acetate
" + Ethyl bromide (Wroczynski and Guye, 1910.)
" + Iodine (Meerum-Terwogt, 1905; Kruyt and Heldermann, 1916.)
41 + Sulfur (Ruff and Winterfeld, 1903.)
TOO grams saturated solution of bromine in carbon disulfide contain 45.4
grams'Br at —95°, 39 grams at - 1 10.5°, and 36.9 grams at - 1 16°.
(Arctowski, 1895 — 1896.)
DISTRIBUTION OF BROMINE BETWEEN WATER AND CARBON TETRACHLORIDE
AT 0°.
(Jones and Hartmann, 1916.)
Gm. Br» per
Gm. CCU
Solution.
Density ,
CCU-Br2.
jms. Bromine per Litei
'• Gm. Brcper
' Gm. CCU.
Solution.
Density /
CCl4-Br2.
Gms. Bromine per Liter.
HzO
Layer.
ecu
Layer.
H20
Layer.
ecu
Layer.
0.01640
1.6454
1.28
26.99
0.07261
1.6896
5-35
122.82
0.01847
1.6470
1.44
30-45
O.o8l62
1.6972
6.03
138.66
0.05433
I-6755
4.12
91.12
0.08661
I.70I2
6.30
184.41
0.06126
1.6809
4-59
103.07
0.1646
1.7667
II .22
29I.IO
161 BROMINE
DISTRIBUTION OF BROMINE AT 25° BETWEEN WATER AND:
(Calculated from results of Jakowkin, 1895. Those in parentheses from Herz and Kurzer, 1910.)
Carbon Disulfide. Bromoform. Carbon Tetrachloride.
Gms. Br. per Liter of; Gms. Br. per Liter of: Gms. Br. per Liter of;
Aq. 'Layer. CS2 Layer. Aq. Layer. CHBr3 Layer. Aq. Layer. CC14 Layer.
0.5 36 (35) o-5 33 0.5 15 (13)
1 80 (75) i 66 i 28 (23)
2 163 (155) 2 136 2 60 (45)
3 240 (230) 3 206 3 90 (70)
4 330 (31°) 4 276 4 123 (95)
5 420 (395) 5 346 5 156 (122)
6 515 (480) 6 415 6 190 (150)
7 620 (565) ... ... 8 260 (220)
10 340 (300)
12 430 (400)
Lewis and Storch (1917) point out that Jakowkin (1896) failed to take into
consideration, the hydrolysis of the bromine in the aqueous phase in the very
dilute solutions. They used o.ooi n HC1 which prevents the hydrolysis but is
presumably too dilute to affect the true solubility. The distribution coefficient
found in this way, given in terms of mols. Br per 1000 gms. H2O, divided by the
mol. fraction of Br in the CC14, is 0.3705 at 25°. These authors also give a series
of determinations of the distribution of bromine between o.i n HBr and CCU
at 25°.
DISTRIBUTION OF BROMINE BETWEEN WATER AND MIXTURES OF CARBON
DISULFIDE AND CARBON TETRACHLORIDE AT 25°.
(Herz and Kurzer, 1910.)
75 Vol. % CS2+25 Vol.
% CC14.
Gms. Bromine per Liter.
Aq. Layer. CS2+CCU Layer.
0.71 46
1.34 87.2
3.98 213.8
5.06 330.5
6.82 444-2
DISTRIBUTION OF BROMINE AT 25° (Herz and Rathmann, 1913) BETWEEN:
Water and Tetrachlorethane. Water and Pentachlorethane.
Grams Bromine per Liter. Gms. Bromine per Liter.
Aq. Layer. CzIfeCU Layer. Aq. Layer. C2H.CU Layer.
0.216 6.47 0.402 10.70
0.592 18.20 0.670 18.29
0.944 29.46 0.864 23.49
1.348 41.65 1.300 35.46
2.444 74-57 2.408 67.44
25 Vol. % CSa + 75 Vol.
% CC14.
Gms. Bromine per Liter.
, 50 Vol. %CSi+5oVol.
% CC14.
Gms. Bromine per Liter.
Aq. Layer.
0.79
i-53
2.32
2.98
3.66
5-26
7-95
9.66
CS2+CCU Layer.
28.4
58.4
86.6
111.3
137.8
205.1
324.9
432.2
Aq. Layer.
0.63
I.I9
I.76
2-45
2-95
6.47
7-97
CS2+CCU Layer.
28.7
54-5
8l.I
II0.9
132.9
343-8
447-7
BROMINE
162
DATA FOR THE DISTRIBUTION OF BROMINE BETWEEN AQUEOUS SALT SOLUTIONS
AND ORGANIC SOLVENTS ARE GIVEN BY THE FOLLOWING INVESTIGATORS:
Immiscible Solvents. t°.
Aqueous CdBrz+CCU 25
Aqueous CdBr2.2KBr+CCl4 25
Aqueous HBr-j-CCL; 25
Aqueous HgBr2+CCLi 25
Aqueous HgBra^KBr-fCCU 25
Aqueous KBr+CCU o
Aqueous KBr-j- €82 32.6
Authority.
(Van Name and Brown, 1917.)
(Lewis and Storch, 1917.)
(Herz and Paul, 1914; Van Name and Brown, 1917.)
(Van Name and Brown, 1917.)
(Jones and Hartmann, 1916.)
(Roloff, 1894.)
BROMOFORM CHBr3.
100 cc. H2O dissolve 0.125 gin. CHBr3 at I5°-2O°.
(Squire and Caines, 1905.)
SOLUBILITY (Freezing-point lowering data, see footnote, p. i) FOR
MIXTURES OF:.
Bromoform and Liquid Carbon Dioxide.
(Biichner, 1905-06.)
Bromoform and Toluene.
(Baud, 1912.)
' Cms. CHBra per
t° of Freezing. ! 100 Cms. Solid Phase.
CHBrs+CeHs.CHs.
+ 7.7
IOO
CHI
-11.4
86.6
(i
— 22.2
75-6
tt
-30.9
69.8
14
-48.5
60.3
11
Gms. CHBrs per
t°. 100 Gms.
CHsBr+C02.
—31 o
-32 3-7
-30 4-9
-16 13-5
- 8 24
- 5 35-2-67.7 quad.pt.
- 3-5 92-1
BRUCINE C2iH20(OCH3)2N202.4H20.
SOLUBILITY OF BRUCINE IN SEVERAL SOLVENTS.
Qnl«»nf t o Gms- Brucine per A.ithnritv
Solvent. t. I00 cms. Sat. Sol.
18-2 2 o . 056-0 . 1 25 (Muller,'i903 ; Squire and Caines, 1905; Zalai, 1910.)
20 12 (Scholtz, 1912.)
1 8-2 2 I . Il-l . 86 (Muller, 1903; Schaefer, 1913.)
0.08 " " .
1.96
Water
Aniline
Benzene
Carbon Tetrachloride 18-22
" " 20
Chloroform 25
Trichlor Ethylene 15
Ether 18-22
Ethyl Acetate 18-22
Ethyl Alcohol 25
Diethylamine 20
Methyl Alcohol 25
Petroleum Ether
Glycerol
Pyridine
ii. 6
2-5
o-75
4.26
45-2
1.6
55-6
(Schindelmeiser, 1901; Gori, 1913.)
(Schaefer, 1913.)
(Wester and Bruins, 1914.)
(Muller, 1903.)
Aq. 50% Pyridine
Piperidene
(Schaefer, 1913.)
(Scholtz, 1912.)
(Schaefer, 1913.)
18-22 0.055-0.088 (Muller, 1903; Zaki, 1910.)
1 8-2 2 2 . 2 (Muller, 1903.)
2O 28 (Scholtz, 1912.)
20-25 21.9 (Dehn, 1917.)
20-25 3T-6 "
20 I (Scholtz, 1912.)
Results for the solubility of brucine and brucine sulfate in mixtures of alcohol,
chloroform and benzene are given by Schaefer (1913).
BRUCINE Per CHLORATE C21H20(OCH3)2N2O2.HC1O4.
loo gms. H2O(+ 2%HC1O4) dissolve 0.15 gm. of the salt at 18°.
(Hofmann, Roth, Hobold and Metzler, 1910.)
163 BEUCINE
BRUCINE SULFATE.
100 cc. methyl alcohol dissolve 0.28 gm. brucine sulfate at 25°. (Schaefer, 1913.)^
" ethyl " " 1.66 " " (Schaefer, 1913.)
" chloroform O.6 (Schaefer. 1913.)
BRUCINE d, /, and i TARTRATE.
SOLUBILITY OF EACH OPTICAL ISOMER IN WATER (Dutiih, 1912.)
Gms. per 100 Cms. Water.
t°. t * \
d Tartrate. I Tartrate. Racemic Tartrate.
20 ... ... 1.38
25 1.008 1.84
35 1-272 3-24
44 1.590 4-64
50 1.854 6.56
BUTANE C4H10.
SOLUBILITY IN WATER AT t° AND 760 MM.
t°. o°. 4°. 10°. 15°. 20°.
Vol. C4Hio per
icovols. H2O 3.147 2.77 2.355 2.147 2.065
DiphenylBUTADIENE.
Freezing-point curves (solubility, see footnote, p. i), are given by Pascal
(1914) for mixtures of diphenylbutadiene and each of the following compounds:
diphenyldiacetylene, diphenylhydrazine and cinnamylidene.
BUTYL ACETATE CHj.C02.CiH9.
SOLUBILITY OF BUTYL ACETATE AND OF BUTYL FORMATE IN MIXTURES
OF ALCOHOL AND WATER.
(Bancroft — Calc. from Pfeiffer — Phys. Rev. 3. 205, '?
cc. H2O added to cause separation of a
Air h 1 second phase in mixtures of the given
in Mixture quantity of alcohol and 3 cc. portions of:
Butyl Formate. Butyl Acetate.
3 3-45 2-°8
6 8.83 6.08
9 14-75 IO-46
12 21.45 J5-37
15 29.65 20.42
18 39.0 25". 60
21 51.8 31.49
24 <*> 37-48
27 43-75
30 50-74
33 59-97
100 cc. H2O dissolve 0.7 cc. isobutyl acetate at 25°. (Bancroft.)
IsoBUTYL ACETATE, etc.
SOLUBILITY IN WATER. (Traube, 1884; at 20°, Vaubel, 1899.)
Grams Com-
* o Compound. pound per zoo
Grams HaO.
22 Iso Butyl Acetate 0.5
22 Iso Butyl Formate x.o
20 Normal Butyric Aldehyde 3 .6
20 Iso Butyric Aldehyde 10.0
BUTYL ALCOHOLS 164
Secondary BUTYL ALCOHOL CH3.CHOH.CH2CH,.
Iso BUTYL ALCOHOL (CH3)2CH.CH2OH.
SOLUBILITY OF BUTYL ALCOHOLS IN WATER, "SYNTHETIC METHOD."
(see Note, p. 16).
(Alexejew, 1886.)
Secondary Butyl Alcohol Iso Butyl Alcohol
and Water. and Water.
Cms. Secondary Butyl Alcohol per too Gms. Cms. Iso Butyl Alcohol per 100 Cms.
Aqueous Alcoholic
Layer. Layer.
13 85
9 84
7-5 83
7 82
7 77
8 72
16 62
28 50
49
Additional determinations of] the reciprocal solubility of secondary butyl
alcohol and water are given by Dolgolenko (1908). This investigator prepared
three fractions of 980-o.8.60, 98.6°-99° and 99°-99.5° boiling point respectively,
and determined the curve for each fraction and water by the "synthetic method."
The first fraction gave a closed curve having both a lower and an upper critical
solution temperature, while the other fractions gave curves with only an upper
critical solution temperature, and in other respects in fair agreement with the
results of Alexejew as shown in the above table. The explanation of this differ-
ence in the case of the first fraction, is supposed to be that this fraction contained
a larger proportion of tertiary butyl alcohol than the others, due to the lower
boiling point of this isomer. Since the tertiary alcohol is entirely miscible
with secondary alcohol and water its presence would restrict the boundaries of
inhomogeneity and, therefore, tend to favor a closed curve for the system.
SOLUBILITIES, DETERMINED BY THE FREEZING-POINT METHOD (see footnote, p. i),
ARE GIVEN FOR THE FOLLOWING MIXTURES CONTAINING BUTYL ALCOHOLS.
Isobutyl alcohol + Water (Dreyer, 1913.)
" + Liquid CO2 (Buchner, 1905-06.)
Normal butyl alcohol + Water (Dreyer, 1913.)
" " " + Liquid CO2 (Buchner, 1905-06.)
Secondary butyl alcohol + Water (Dreyer, 1913; Timmermans, 1907, 1910, X9«.)
}" " + " + Hydroquinine (Timmermans, 1907.)
Tertiary butyl alcohol -f Water. (Dreyer, 1913.)
Aqueous
Alcoholic
*
Layer.
Layer-
— 20
27
66
— 10
28
60
0
27-5
56
10
26.0
57
20
22-5
60
30
18
63-5
40
16
65-5
6o
13
67
80
IS
63
100
20
52
io7crit.
temp. 33
120
130
133 crit. ternp.
1 65 IsoBUTYL ALCOHOL
DISTRIBUTION OF ISOBUTYL ALCOHOL BETWEEN WATER AND COTTON SEED
OIL AT 25°. (Wroth and Reid, 1916.)
Cms. C4H9OH per TOO cc. Cms. C«H»OH per too cc.
OU Layer. HZO Layer. Ratio. [Oil Layer. H2O Layer. - Ratio
1.168 2.043 i-74 1-375 2-3oi 1.67
1.276 2.250 1.76 1-405 2.429 1.72
1.288 2.135 X-6S x-495 2-45o 1-64
The partition coefficient of tertiary butyl alcohol (CH3)2C(OH)CH3, between
olive oil and water is given as 0.176 at ord. temp. (Baum, 1899.)
IsoBUTYLAMINE HYDROCHLORIDE (CH3)2CHCH2NH2.HC1.
IOO gms. H2O dissolve 238.9 gms. of the salt at 25°. (Peddle and Turner, 1913.)
IOO gms. CHC18 dissolve 11.56 gms. of the salt at 25°. (Peddle and Turner, 1913.)
BUTYLCHLORAL CH3CHC1.CC12CHO.
The distribution coefficient of butylchloral between oil and water is given as 1.6.
(Meyer, 1907.)
BUTYLCHLORALHYDRATE CH3CHC1.CC12.CH(OH)2.
100 gms. H2O dissolve 2.7 gms. butylchloralhydrate at 15.5°
(Greenish and Smith, 1903.)
2.3 " " at I5°-20°.
(Squire and Caines, 1905.)
glycerol " 100 " " at I5°-2O°.
(Greenish and Smith, 1903.)
The partition coefficient of butylchloralhydrate between olive oil and water is
given as 1.589 at ord. temp. (Baum, 1899.)
BUTYRIC ACIDS (normal) CH3(CH2)2COOrJ; (iso) (CH3)2CH.C6OH.
SOLUBILITY OF NORMAL BUTYRIC ACID IN WATER, DETERMINED BY THE
FREEZING-POINT METHOD. (Faucon, 1909, 1910.)
t-of Gms. Acid per f. of Gms. Acid per t<> of Gms. Acid per 100
Congealing. Congealing. ' Congealing. Gms. Mixture
oo— 3.57 67.38 —13-40 87.62Eutec.
— i. 08 5.12 — 5.20 75 —12.40 90.08
— 2.70 12.75 — 6.80 80 —10 95 .92
— 2.96 25.32 — 8.61 84 — 8 98.60
-3.07 50.60 -10.25 85.41 - 5.40 99.15
-3.14 59.72 -12.54 86.54 - 3.12 loo
Higher values for the temperature of congealing of the above mixtures are
given by Ballo (1910). For additional data see also Timmermans (1907) and
Tsakalotos (1914). Data for the miscibility of normal butyric acid and water
are also given by Faucon. The curve is entirely in the metastable region. The
mixtures are either opalescent or completely homogeneous and never form two
distinct layers, even with the application of centrifugal force. The results are
as follows:
t° of opalescence —5.2 —4.2 —4 — 3.8crit. t. —4-5 — 7
Gms. acid per 100
v gms. mixture 25 30 35 40 50 58 . 2
SOLUBILITY OF ISOBUTYRIC ACID IN WATER, DETERMINED BY THE FREEZING-
POINT METHOD. (Faucon, 1910.)
The congealing temperatures for mixtures containing up to 60 grams iso-
butyric acid per ipo gms. coincide with the results given in the above table for
normal butyric acid and water. For higher concentrations the following results
were obtained.
t° of congealing -3.09 —3-35 ~3-6i -12.5 -80
Gms. acid per 100
gms. mixture 70.10 82.08 86.44 97-21 IO°
BUTYRIC ACID
166
MlSCIBILITY OF ISOBUTYRIC ACID AND WATER, DETERMINED BY THE
"SYNTHETIC METHOD."
(Smirnoff, 1907.)
Gms. "Acid per 100 Gms.:
10.05
12
14
16
18
20
22
22.5
23
Upper Layer.
Lower Layer.
69.08
17.82
67.I
18.3
64.9
I9.I
62.3
20
59-2
21. 1
55-4
22.8
49
25.8
46
27
4i
29
34-7
Determinations varying more or less from the above are given by Rothmund
(1898), Friedlander (1901) and Faucon (1910). The discrepancies are shown by
Smirnoff to be due to the effect of variations in purity of the isobutyric acid upon
the position of the curve. Smirnoff fractionated the purest obtainable acid and
determined the miscibility curve for each fraction. The above results were
obtained with fraction 4 of boiling point 154°-! 55°, twice refractionated.
An extensive series of determinations are* given by Smirnoff of the effect of
various percentages o£ different salts upon the temperature of immiscibility of
aqueous 16.46% isobutyric acid solution.
DISTRIBUTION OF BUTYRIC ACID BETWEEN WATER AND BENZENE AT I3°-I5°
(Georgievics, 1913.)
Gms. Acid Found per-
Gms. Butyric Acid
Used.
2.0044
2.9968
3.5028
4.0088
4-5342
150 cc.
Benzene Layer.
1.7643
2.6965
3-I740
25 cc.
HzO Layer.
o . 2401
0.3003
0.3288
0-3544
0.3821
4-I52I
The distribution ratio of normal butyric acid between water and benzene at
room temperature was found by King and Narracott (1909), to be I to 0.7585,
and for isobutyric acid, the ratio was I to 0.810.
One determination of the distribution of butyric acid between sat. aqueous
CaCl2 solution and kerosene gave 7.2 gms. acid per 100 gms. aqueous layer and
92.8 gms. per 100 gms. kerosene layer at ord. temp. (Crowell, 1918.)
DATA FOR THE FOLLOWING TERNARY SYSTEMS CONTAINING NORMAL
BUTYRIC ACID ARE GIVEN BY TIMMERMANS, 1907.
Normal Butyric acid + Water + Azobenzene.
+ Barium nitrate.
+ Benzophenone.
-j- Camphor.
+ Cane sugar.
-j- Mannite.
-j- Naphthalene.
+ Potassium sulfate.
+ Sodium chloride.
Freezing-point data are given for mixtures of n butyric acid and formamide by
English and Turner (1915), and for mixtures of trichlorobutyric acid and dimethyl
pyrone by Kendall (1914).
167 CADMIUM BROMIDE
CADMIUM BROMIDE CdBr,.
SOLUBILITY IN WATER.
(Dietz — Ber. 32, 95, '99; Z. anorg. Chem. 20, 260, '09; Wiss. Abh. p.t. Reichanstalt, 3, 433, 'oo; see also
Eder — Dingier polyt. J. 221, 189, '76; Etard — Ann. chim. phys. [7] 2, 536, '94.)
Gms.CdBr2 Mols. CdBr2 Gms. CdBr2 Mols. CdBr2
t°. per ioo Gms. per ioo Solid Phase. t°. per ioo Gms. per ioo Solid Phase.
Solution. Mols. H2O. Solution. Mols. H2O.
o 37.92 4.04 CdBr2.4H2O 40 60.65 10.20 CdBr2.H2O
18 48.90 6.21 45 60.75 10.24
30 56.90 8.73 60 61.10 10.39
38 61.84 10.73 80 62.29 10.48
35 60.29 10.05 CdBr2.H2O ioo 61.63 .10.63
Density of saturated solution at 18°= 1.683.
SOLUBILITY OF CADMIUM BROMIDE IN ALCOHOL, ETHER, ETC.
ioo gms. sat. solution of CdBr2.4H2O in abs. alcohol contain 20.93 gms- CdBr2
at 15°. (Eder.)
ioo gms. sat. solution of CdBr2.4H2O in abs. ether contain 0.4 gm. CdBr2 at 15°.
(Eder.)
ioo gms. absolute acetone dissolve 1.559 gms. CdBr2 at 18°. dj^ sat. sol. =
0.8073. (Naumann, 1904.)
ioo gms. benzonitrile dissolve 0.857 gm. CdBr2 at 18°. (Naumann, 1914.)
ioo gms. anhydrous hydrazine dissolve 40 gm. CdBr2 at room temp.
(Welsh and Broderson, 1915.)
RECIPROCAL SOLUBILITIES, DETERMINED BY THE METHOD OF LOWERING OF THE
FREEZING-POINT (see footnote, p. i), ARE GIVEN FOR THE FOLLOWING MIXTURES:
Cadmium Bromide + Cadmium Chloride (Nacken, 1907; Ruff and Plato, 1903.)
-j- Cadmium Iodide (Nacken, 1907.)
+ Calcium Fluoride (Ruff and Plato, 1903.)
+ Cuprous Bromide (Herrmann, 1911.)
-j- Potassium Bromide (Brand, 1913.)
+ Sodium Bromide
+ " + Potassium Bromide "
CADMIUM (Mono)AMMONIUM BROMIDE CdBr2.NH4Br
SOLUBILITY IN WATER.
(Rimbach, 1905; Eder.)
ioo Grams Solution contain Gms. Atomic Relation. G. CdBr2.NH4Br
(1 .
Cd.
Br.
NH4.
'Cd :
Br :
NH*.
per ioo Lri
Solution.
i.o
16.33
34.87
2.63
I
3
I
53-82
14.8
17.40
37-15
2.80
I
3
I
58.01
52.2
19.79
42.38
3-21
I
3
I
65.3I
no. i
22.99
49.17
3-72
I
3
I
75.98
ioo gms. sat. solution of CdBr2.NH4Br in abs. alcohol contain 15.8
gms. double salt at 15° (Eder).
ioo gms. sat. solution of CdBr2.NH4Br in abs. ether contain 0.36
gm. double salt at 15° (Eder).
CACODYLXC ACID (CH3)2AsO.OH.
ioo cc. H2O dissolve about 200 gms. cacodylic acid at 15°. (Squire and Caines, 1905.)
ioo cc. 90% alcohol dissolve about 28.5 gms. cacodylic acid at 15°. " "
CADMIUM BROMIDE
168
CADMIUM (Tetra) AMMONIUM BROMIDE CdBr2.4NH4Br.
SOLUBILITY IN WATER.
(Rimbach.)
The double salt is decomposed by water at temperatures below 1
ioo Gms. Solution contain Gms
t>
*
Cd.
Br.
NH4. Cd
: Br : NH4. *
Cd :
Br ;
; NH4. "
0
.8
14.72
50.46
6.67 I
4
.82 2
.82
I 10.02
8.02
13
•o
14-95
51 .48
6.85 I
4
-85 2
•85
I II
•57
9-57
44.0
15 -OI
53-85
7-35 i
5
•04 3
.04
I
6
.84
4.84
76
•4
14.6
55-28
7.80 I
5
•32 3
•32
I
6
•63
4-63
123
•5
15 .5
59-50
8.45 I
5
•38 3
•38
I
7
.40
5-40
1 60
.0
14-7
62.67
9-43 i
5
•99 3
•99
I
6
•03
4-03
CADMIUM (Mono) POTASSIUM
BROMIDE
CdBr2.
KBr.H2O.
SOLUBILITY
IN
WATER.
(Rimbach; see also Eder.)
*o
ioo Gms. Solution
contain Gms.
Atomic Relation in Sol.
Gms.CdBr2.KBr
*
Cd. Br. K.
Cd :
Br
: K.
Solution.
0
•4
IS-
4i 33-
o 5.42
I
3
I
53-63
JL5
.8
16.
85 35-
96 5.86
I
3
I
58.61
5°
• O
19.
58 41.
86 6.85
I
3
I
67-87
112
•5
22 .
24 48.
28 8.14
0.98
3
1.03
78.11
CADMIUM TetraPOTASSIUM BROMIDE is decomposed by water at
ordinary temperatures.
CADMIUM (Mono)RUBIDIUM BROMIDE CdBr2.RbBr.
SOLUBILITY IN WATER.
(Rimbach.)
to
ioo Gms.
Solution contain Gms. Atomic Relation in Sol. Gms. CdBrz.RbBr
.
Cd.
Br.
Rb.
' Cd :
Br
: Rb.'
Solution.
o
4
8-37
17-93
6-43
I
3
1. 01
32.
65
14
•5
10,
,72
23.02
8.30
O.
99
3
I .OI
41.
87
49
.2
15.01 32.13
11.51
I
3
I
58.
54
107
•5
19.65
41.12
14.06
I.
02
3
0.96
75-
77
CADMIUM
(Tetra)RUBIDIUM
BROMIDE
CdBr2.4RbBr.
SOLUBILITY IN WATER.
(Rimbach.)
^0 ioo Gms. Solution contain Gms. Atomic
Relation in Sol. ^
per ioo Gms.
Solution.
' Cd
Br
Rb.
'Cd
: Br
: Rb.
0
-5
5
.70
24.94
17.97
0.
98
6
4-05
47-
95
13
•5
6
•55
28.74
20.74
0.
97
6
4-05
55-
17
•5
8
•25
35-51
25-39
0.
99
6
4.O2
68.
82
114
•5
9
•50
40.67
29.0O
I .
00
6
4.0
79-
04
169
CADMIUM BROMIDE
CADMIUM (Mono) SODIUM BROMIDE CdBra.NaBr2jH,O.
SOLUBILITY IN WATER, ETC., AT 15°.
(Eder — Ding, polyt. J. 221, 189,' '76.)
Solvent.
Gms. CdBr2.NaBr per 100 Cms.
Solution. Solvent.'
Water 49 -o 96.1
Absolute Alcohol 21.2 27.0
Absolute Ether 0.52 0.53
Solid
Phase.
CdBr2.NaBr.2iH2O
CADMIUM CHLORATE Cd(ClO3)2.2H2O.
SOLUBILITY IN WATER.
(Meusser, 1902 )
Gms.
- 6.5
-I3.0
— 2O.O
-15.0
Solution.
26.18
52.36
72.10
72.53
Mols.
Gms.
to Cd(ClO»)z
" ' per 100 Gms
Mols.
Cd(C103)2 solid Phase.
. per 100
er i£b. ° j
Solution.
Mols. H2O.
3
.07
Ice
db
O
74
•95
25
.92
Cd(ClO3)2.2HzO
9
•52
"
18
76
.36
27
.98
'*
22
.47 Cd(ClO3)2.2HiO
49
80
.08
34
.82
M
22
.87
65
82
-95
42
.14
"
;. solution
at 18° = 2
.284.
CADMIUM CHLORIDE CdCl2.2|H2O.
SOLUBILITY IN WATER.
(Dietz — W. Abh. p. t. Reichanstalt 3, 433, 'oo; above 100°, Etard — Ann. chim.phys.fr] 2, 536, '94.)
G. CdCl2 per Mols.CdCl2 ~ ,. .
t °. 100 Gms. per 100 ^T
Solution. Mols.H2O. Phase'
G.CdCljper
t °. loo Gms.
Solution.
- 9
43
•S8
7
•5"
+ 10
57
•47
0
+ 10
49
55
•39
•58
9
12
.6
•3
•CdCI2.4H20
20
40
57
57
•35
5i
15
59
.12
14
.2.
60
57
•7i
— 10
44
•35
7
.8"
80
58
.41
o
47
•37
9
• O
100
59
•S2
+ 18
52
•53
10
•9
•CdCI2.2iH2O
150
64
.8
30
56
.91
12
.8
(monoclinic)
200
72
• 0
36
57
.91
13
•5.
270
77
•7
Mols.CdCl,
per TOO
Mob.H,0.
13.2
13-3
13-4
13.8
14. 4J
Density of saturated solution at 18° = 1.741.
Solid
PV,~<M
Phase'
100 gms. abs. ethyl alcohol dissolve 1.52 gms. CdCl2 at I5°.5.
100 gms. abs. methyl alcohol dissolve 1.71 gms. CdCl2 at i5°-5. (de Bruyn, 1891.)
loo gms. abs. methyl alcohol dissolve 1.5 gms. CdCl2 at the crit. temp.
(Centnerszwer, 1910.)
ioo gms. benzonitrile dissolve 0.063 gm. CdCl2 at 18°. (Naumaan, 1914.)
CADMIUM CHLORIDE
170
RECIPROCAL SOLUBILITIES, DETERMINED BY THE METHOD OF LOWERING OF
THE FREEZING-POINT (see footnote, p. i), ARE GIVEN FOR THE FOLLOWING
MIXTURES:
Cadmium Chloride + Cadmium Iodide
" " + Cadmium Fluoride
+ Cadmium Sulfate
+ Calcium Chloride
" " + Cuprous Chloride
" + Lead Chloride
(Nacken, 1907 (c); Ruff and Plato, 1903.)
(Ruff and Plato, 1903)
(Sandonnini, 1911, 1914; Menge, 1911.)
(Herrmann, 1911.)
(Sandonnini, 1912, 1914; Herrmann, 1911.)
+ Magnesium Chloride (Menge, 1911.)
-f- Manganese Chloride (Sandonnini, 1914; Sandonnini and Scarpa, 1911.)
-j- Mercuric Iodide (Sandonnini, 1912.)
•f- Potassium Chloride (Brand, 1911.)
-j- Sodium Chloride
+ " . " + Potassium Chloride (Brand, 1911.)
+ Strontium Chloride (Sandonnini, 1911; 1914.)
+ Thallium Chloride (Korreng, 1914; Sandonnini, 1913.)
-j- Tin (ous) Chloride (Herrmann, 1911; Sandonnini, 1914.)
4" Zinc Chloride (Herrmann, 1911.)
CADMIUM AMMONIUM CHLORIDE CdCl2.NH4Cl.
SOLUBILITY IN WATER.
(Rimbach — Ber. 30, 3075, 1897.)
IPO Gms. Solution contain Cms. Gms. CdCl2.NH*Cl per 100 Cms.
* .
'Cd.
Cl.
NH.
'Solution.
Water.
2.4
14.26
13-44
2.24
29.94
42.74
16.0
15.82
I5-07
2.56
33-45
50.26
41.2
18.61
17.46
2.89
38.96
63-83
63.8
20.92
J9-73
3-34
43-99
78-54
105.9
24.70
23-52
4.01
52-23
109-33
OADMIUM (Tetra) AMMONIUM CHLORIDE CdCl2.4NH4Cl.
IN CONTACT WITH WATER.
The salt is decomposed in aqueous solution.
(Rimbach.)
100 Gms. Solution contain Gms.
Atomic Relation in Solution.
V •
' Cd.
Cl.
NH*.
Cd
: Cl :
NH*:
3-9
5-75
18.17
7-37
i
9.96
7.96
16.1
6.96
20.26
7-97
i
9-20
7-13
40.2
9.91
23.84
8.92
i
7.6l
5-61
58.5
12.50
26-53
9-35
i
6.7I
4.66
112.9
16.66
3r-79
10.78
i
6.02
4-02
H3-9
16.51
32.71
11.30
i
6.26
4.26
SOLUBILITY OF MIXTURES OF CADMIUM TETRA AMMONIUM CHLORIDB
AND CADMIUM AMMONIUM CHLORIDE IN WATER.
(Rimbach — Ber. 35» 1300, '02.)
4.0
100 Gms. Solution contain Gms.
Atomic Relation.
Solid Phase,
Mol. per cent of:
• .
Cd.
Cl.
NH*.
Cd
: Cl :
NH*.
CdCl,.
NH*C1.
CdClj.
4NH4C
I.I
5-34
17.62
7.27
I
10-47
8.50
49.6
50-4
14.0
7.12
19.86
7.84
I
8.84
6.87
47-o
53-o
40-7
10.24
23.82
8.85
I
7-37
5-37
77-0
23-0
58.5
12.50
26.53
9-35
I
6.71
4.66
...
...
171 CADMIUM CHLORIDE
SOLUBILITY OP MIXTURES OF CADMIUM TETRA AMMONIUM CHLORIDE
AND AMMONIUM CHLORIDE IN WATER.
(Rimbach.)
100 Cms. Solution Atomic Solid Phase,
$0^ contain Gms. Relation. Mol. per cent of:
Cd. Cl. NH". Cd : Cl' : NIL,. ' Nt^Cl. CdCl2.4NH«Cl.
i.o 2.82 17.11 7.82 i 19.21 17.28 59.0 41.0
13.2 2.76 18.84 8.71 i 21.62 19.62 74-o 26.0
40.1 3.16 22.56 10.49 l 22.65 20.74 71.0 29.0
58.2 3.51 25.21 11.72 i 22.79 20.89 69.0 31.0
CADMIUM BARIUM CHLORIDE 2(CdCl2).BaCl2.sH2O.
SOLUBILITY IN WATER.
(Rimbach — Ber. 30, 3083, '97.)
t°.
100 Gms. Solution
contain Gms.
Gms. 2(CdCl2).BaCl2
per 100 Gms.
Cd.
Cl. Ba.
Solution. Water.
22.6
17.71
16.89 ii. o
45-60 83.82
41-3
19.22
18.15 11.77
49.14 96.62
53-9
I9-85
18.75 12.41
51.04 104.25
62 .2
20-59
19.66 12.83
53.08 II3-I3
69-5
21 .20
20. 18 13-09
54.47 119.64
IO7 -2
24.25
23.23 14.90
62.38 165.85
CADMIUM
BARIUM CHLORIDE CdCl
2.BaCl2.4H20.
SOLUBILITY IN WATER.
(Rimbach.)
100 Gms. Solution
Gms. CdCl2.BaCla
t».
contain Gms.
per loo Gms.
Cd.
Cl. Ba.
Solution. Water.
22.5
11.98
15.19 14.71
41.88 72.06
32-9
12.40
16.18 16.09
44.67 80.73
41.4
I3-05
16.95 16.81
46.81 88.01
53-4
13.96
18.21 18.13
50.30 101.21
62.0
14-73
18.81 18.74
52.28 109.56
97-8
17-57
22.48 22.00
62.05 163.50
108.3
18-53
23.51 22.79
64.83 184.33
109.2
18.67
23.69 29.95
65.31 188.27
CADMIUM MAGNESIUM CHLORIDE 2(CdCl2)MgCl2.i2HA
SOLUBILITY IN WATER.
(Rimbach.)
100 Gms. Solution
t». contain Gms.
Gms. 2(CdCl2).MgClj
per 100 Gms.
2.4
20-8
45-5
67.2
121. 8
Cd.
22 .14
24.30
26.24
28.45
31.84
Cl.
21 .06
22.80
24-55
26.71
30.20
Mg.
2.41
2-55
2 .72
2-98
3-44
Solution.
45.6l
49.69
53-51
58.14
65.48
Water.
83.86
98.77
115.10
138.90
189.69
CADMIUM CHLORIDE
172
CADMIUM (Mono)RUBIDIUM CHLORIDE CdCl2.RbCl.
SOLUBILITY OF CADMIUM MONORUBIDIUM CHLORIDE IN WATER.
(Rim bach, 1902.)
1.2
14-5
41.4
57-6
103.9
ioo Gms. Solution contain Gms.
Cms. CdCl2.RbCl per ioo Gms.
Cd.
Cl.
Rb. ^
Solution.
Water.
4.80
4-53
3^3
I2.Q7
14.90
6.20
5.88
4-75
16.80
2O.I9
9-34
8.86
7-14
25-31
33.89
11.40
10.78
8.63
30-83
44.58
17.14
16.37
J3-39
46.62
87.36
CADMIUM (Tetra)RUBIDIUM CHLORIDE CdCl2.4RbCL
IN CONTACT WITH WATER.
(Rimbach.)
• The double salt decomposes to CdCl2.RbCl and RbCl.
t ° .
100 Gms.
Solution contain
Gms.
Atomic Relation.
Solid Phase,
Mol. per cent of:
Cd.
Cl.
Rb.
Cd
:
Cl
: Rb.
CdClo.
RbCl.
CdCl2.
4RbCl.
0.7
0.65
6.52
14
•73
I
31
.88
29
.88
30
70
8.8
1.07
7-37
16
•!3
I
21
.89
!9
.89
24
76
13.8
1.32
7.86
16
•93
I
18
.88
16
•83
16
84
42.4
3-21
"•35
22
•45
I
II
.21
9
.21
14
86
59-o
4.61
i3-4i
25
•31
I
9
•23
7
•23
33
67
108.4
8.94
18.57
31
•*5
I
6
•57
4
•59
SOLUBILITY OF MIXTURES OF CdCl2.4RbCl AND RbCl IN WATER.
(Rimbach.)
0-4
14.8
17.9
ioo Gms. Solution contain Gms.
Cd.
Cl.
12.86
13.62
I4-O
Rb.
30-97
32-8I
33-71
Atomic Relation.
Cd
Cl : Rb.
I I
I I
I I
Solid Phase,
Mol. per cent of:
CdCl2.4RbCi RbCl.
55 45
67 33
80 20
THE EFFECT OF THE PRESENCE OF HC1, CaCl2 AND OF LiCl UPON THE DECOMPO-
SITION OF CADMIUM TETRARUBIDIUM CHLORIDE BY WATER AT 16°.
(Rimbach, 1905.)
ioo Gms. Solution contain Gms.
Mols. per ioo Mols. H2O. Molecular Ratio.
Total Cl.
Cl.
HCl.
Cd.
Rb.
CdCl2.
RbCl.
HCl. CdCl2 : K
bCl.
36.44
0.84
36.61
0.41
i-39
O
.109
O
483
29.76
4
•43
28.45
0.80
28.44
o-35
1-38
O
.082
0
422
20.35
5
•JS
12.09
3-24
p.II.
0.69
6.74
O
•139
I
772
5.60
12
•75
Ca.
CaCl2.
CaCl2.
14.98
7-56
20.91
o-73
2.80
O
.159
0
•799
4-59
5
.04
12.70
5-77
15.96
0.77
4.87
O
.163
I
•353
3-41
8
.31
10.85
3-78
14.47
1. 00
8.51
O
.211
2
•365
2.24
ii
.22
9.08
1.84
5-10
1.24
12 .14
O
.262
3
•385
1.09
12
.92
Li.
LiCl.
LiCl.
26.49
4.87
29.40
0.56
3-871
O
•139
I
.271
19.40
9
.13
20-37
3-33
2O -II
0.52
7.84
0
.122
2
•433
12.54
19
.88
See Note on next page.
173
CADMIUM CHLORIDE
CADMIUM (Mono) POTASSIUM CHLORIDE CdCl2.KCl.H2O.
SOLUBILITY IN WATER.
(Rimbach— Ber. 30, 3079, '97; see also Croft — Phil. Mag. [3] 21, 356, '42.)
ioo Gms. Solution
$o_ contain Gms.
2.6
Cd.
9-53
11.63
Cl.
9-03
10.98
K.
3-31
3-99
41-5
60.6
I05.I
15-47
17.68
22.46
14-73
16.80
21.34
5-45
6. 20
7.87
Cms. CdCb.KCl
per 100 Gms.
Solution.
21.87
26.60
35-66
40.67
5J-67
Water.
27.99
36.24
55-34
68-55
106.91
CADMIUM (Tetra) POTASSIUM CHLORIDE CdCU^KCL
IN CONTACT WITH WATER.
(Rimbach.)
The double salt is decomposed when dissolved in water at ordinary
temperature.
ioo Grams Solution contain Gms.
C
4
23 .6
50.2
108.9
t°.
Cd.
Cl.
K.
3.64
9.84
8.31
5-66
14.02
11.52
9.10
18.09
13.60
11.94
23.11
17.16
NOTE. — The effect of the presence of certain chlorides upon the
decomposition of cadmium tetra potassium chloride by water at 16°
was investigated by Rimbach in a manner similar to that used in the
case of cadmium tetra rhubidium chloride (see preceding page). The
results, which show the extent to which increasing amounts of the
several chlorides force back the decomposition of the double salt, were
plotted on cross-section paper, and the points at which the decom-
position was prevented, were determined by interpolation. These
values which show the minimum amount of the added chlorides which
must be present to insure the crystallization of the pure double salt are
shown in the following table.
Added
Chloride.
Mols.
per
ioo Moli
5. H2<
L).
Density of
Solutions.
Mols.
per
Liter of !
Solution.
CdCl2.
KC1.
Added]
Chloride.
CdCl2.
KC1.
Added"
Chloride.
HC1
0.074
0
.296
19
.80
I
.1403
0-033
O
.132
8.828
LiCl
0-344
X
•376
9
•30
I
.1380
0.166
o
.663
4-483
CaCl,
0-544
a
.I76
3
.80
I
•2333
0.270
X
.080
1.887
KC1
1.034
6
•5*4*
2
•378
I
.214
0.507
3
.195*
1.167
* Total.
CADMIUM CHLORIDE
174
SOLUBILITY OF CADMIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AT SEVERAL TEMPERATURES AND VICE VERSA. (Sudhaus, 1914.)
Gms. per 100 gms. H2O.
Solid Phase.
Gms. per 100 gms. HzO.
Solid Phase.
'CdCh.
KCL'
CdCh.
KCL '
Results at
i9-3°.
Results at
40.1°.
in- 3
o.o
CdCl2.2|H2O
133.85
O.O
CdCl2.H2O
59-59
6.7
" -j- DM-I
92.15
2.70
" + DI.M
*26.98
11.09
DI.I.I
51.90
11.50
DI.I.I
n. 61
30.04
" + DL4
*37-9i
15.21
"
1.44
34.76
DL4+KC1
24-45
21.73
tt
o.o
33-94
KC1
18.97
35-51
"
Results at
29.7°.
19.92
37-63
" +D,.4
129.65
o.o
CdCl2.2jH20
2.98
40.45
Di.4+KCl
97.62
0.70
a
o.o
40.36
KC1
68.23
7.08
"~\~ DI.I.I
Results at
54-5.
47.12
9.89
DI.I.I
133.9
0.0
CdCl2.H2O
*32.67
13.06
(t
102.15
2.32
" +DM.I
24.26
16.10
"
*44.oi
18.39
DI.I.I
15-99
25-97
"
26.13
43.78
" +Di.4
15-47
33.58
" + DL4
4.20
45-52
Di.4+KCl
2.42
37-66
DL4+KC1
o.o
43.00
KC1
o.o 37.21
DI.I.I = CdCl2.KCl.H2O,
KC1
Di.4 = CdCl2.4KCl.
)ws; the solubility of the double salt in water.
SOLUBILITY OF THE DOUBLE SALT. CdCl2.4KCl IN WATER.
(Sudhaus, 1914.)
19-3
23-6
29.7
40.1
50.2
54-5
Gms. CdCl2.4KCl per
100 gms. HzO.
41.65
45-35
49-05
57-55
68.89
69.91
Mol. Ratio in Solution.
iCdC!2
6.37KC1
5-85 "
5-34 "
4.60 "
4.30 "
4.12 "
SOLUBILITY OF CADMIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE
AT SEVERAL TEMPERATURES AND VICE VERSA. (Sudhaus, 1914.)
Gms. per 100 gms. HjO.
Solid Phase.
CdCl2.2|H2O
" +DL,.,
Di.2.3
u
" +NaCl
NaCl
CdCU. NaCl.
Results at 19.3°.
111.30 o.o
116.64 7-52
85.15 12.19
*40.oi 25.67
5.96 36.76
o.o 35.84
Gms. per too gms.
Solid Phase.
Results at 29.7°.
CdCl2. NaCl.
Results at 29.7° (con.).
*43-74 27.46 Di.2.3
9.43 37-54 " +NaCl
Results at 40.1°.
137.03 15.14 CdCl2.H2Of-D1.2.3
*48.i7 29.50 Di.2.3
13.31 38.16 +NaCl
Results at 54.5°.
9.63 CdCl2.2jH20+Di.2.3i4o.42 19.10 CdCl2.H2O+Di.2.3
Di.2.3
*52-76
22.53
o.o
32.97
39-07
36.82
132.67
123.54 10.10
106.16 12.92
91.10 15.41 "
Di.w = CdCl2.2NaCl.3H20.
* Shows the solubility of the double salt in water.
CADMIUM CINNAMATES (C6H5CH:CH.COO)2Cd.
100 gms. water dissolve 0.070 gm. cadmium cinnamate at 26°.
loo 0.56 ' cadmium isocinnamate at 20°.
100 " " " o.io " cadmium allocinnamate at 20°
Di.2-3
" +NaCl
NaCl
(de Jong, 1909.)
(Michael, 1903.)
175
CADMIUM CYANIDE
CADMIUM CYANIDE Cd(CN)2.
100 gms. H2O dissolve 1.7 gms. Cd(CN)2 at 15°.
Qoannis, 1882.)
CADMIUM FLUORIDE CdF2.
loo cc. of sat. solution in water contain 4.33 gms. CaF2 at 25°.
100 cc. of sat. solution in 1.08 n. HF contain 5.62 gms. CaF2 at 25°. Qaeger, 1901.)
jFreezing-point lowering data (solubility, see footnote, p. i) are given for mix-
tures of cadmium fluoride and cadmium iodide by Ruff and Plato (1903), and
for mixtures of cadmium fluoride and sodium fluoride by Puschin and Baskov,
(1913).
CADMIUM HYDROXIDE Cd(OH)2.
SOLUBILITY IN WATER.
I liter of aqueous solution contains 0.0026 gm. Cd(OH)2 at 25°.
(Bodlander, 1898.)
SOLUBILITY IN AQUEOUS AMMONIUM HYDROXIDE SOLUTIONS.
Results at 25°. Results at 16-21°.
(Bonsdorff, 1904.) (Euler, 1903.)
Normality of
NHs.
i.o
1.8
4.6
Gms. Cd(OH)z
per liter.
0.274
0.707
I.5l6
5.609
16-17
21
u
Normality of
NHs.
Gms. Cd(OH)2
per liter.
0.47
0.87
0.26
0.44
I.I7
0-51
0.32
CADMIUM IODIDE CdI2.
SOLUBILITY IN WATER.
(Dietz, 1900; see also Kremers, 1858; Eder, 1876; Etard, 1894.)
Gms. CdI2 per too Gms. M°k- CdI2
^0 Gms. Cdl2 per 100 Gms.
Mols. Cdli
Solution. Water. Mols. HjO.
Solution. Water.
per 100
Mols. H2O.
o 44.4 79.8 3.9
30 47.3 89.7
4-43
10 45.4 83.2 4.1
40 48.4 93.8
4.6
15 45.8 84.5 4.17
5° 49-35 97-4
4.8
18 46.02 85.2 4.2
75 52.65 in. 2
5-4
20 46.3 86.2 4.26
100 56.08 127.6
6-3
*2S 46.8 87.9 4.34
Density of saturated solution at 18
0 = 1.590.
SOLUBILITY OF CADMIUM
IODIDE IN ORGANIC SOLVENTS.
"Solvent t° G^-
Cdlj per loo Gms.
Solution. Solvent/
Absolute Alcohol 15 50
.5 I O2 (Eder.)
Ethyl Alcohol 20 42
.6 74 . 27 (Timofeiew, 1891.)
Methyl Alcohol 20 59
.O 143.7 (Timofeiew, 1891.)
Propyl Alcohol 20 28
.9 40 . 67 (Timofeiew, 1891.)
Absolute Acetone 18 20
25 * (Naumann, 1904.)
Benzonitrile 18
I . 63 (Naumann, 1914.)
Ethyl Acetate 18
I . 84 | (Naumann, 1910.)
Ethyl Ether 12°
0.143 (Tyrer, 1911.)
Anhy. Hydrazine 15-20
84 J (Welsh and Broderson, 1915.)
Benzene 16.0
0 . 047 (Linebarger, 1895.)
35.0
0.094
?(fca=.994. \d
is =.9145- tperioocc.
CADMIUM IODIDE 176
SOLUBILITY OF CADMIUM IODIDE IN METHYL ALCOHOL, ETHYL ALCOHOL, PROPYL
ALCOHOL AND IN ISOPROPYL ALCOHOL AT DIFFERENT TEMPERATURES.
(Muchin, 1913, see also Timofeiew, 1894.)
Grams Cdl2 per 100 Grams Sat. Solution in:
.• •
CHaOH.
CtHsOH.
CsHvOH.
C3H7OH(iso).
0
67
33-5
16
36.9
5
. . .
4i
22
36-9
10
68
54 (at 1 2 .6° = tr. temp.)
28.5
37-2
20
69
53
41 . 5 (tr. temp.)
37-3
25
69-5
52.2
37-8
37-3
30
70
51 .5
35-5
37-3
40
7i
50.8
34-5
37-3
So
72-5
50
34-o
37-3
SOLUBILITY OF CADMIUM IODIDE IN ETHYL ETHER. (Linebarger, 1895.)
f o Mols Cdlz per Gms. CdI2
100 Mols. CdIi+(C2Hs)2O. 100 gms.
o 0.03 0.148
15.5 0.04 0.198
20-3 0.05 0.247
SOLUBILITY OF CADMIUM IODIDE IN METHYL FORMATE, ETHYL FORMATE, PROPYL
FORMATE AND INJETHYL ACETATE AT DIFFERENT TEMPERATURES. (Muchin, 1913.)
Gms. CdI2 per 100 Gms. Sat. Solution in:
l> .
HCOOCHs.
HCOOCzHs.
HCOOC3H7.
CH3COOC2H5.
0
0.84
1.16
2-37
4-73(?)
13.0
o-75
1.05
2.07
1.67
26.0
0.66
0.77
i-53
2.02
CeHsNHz.
CsHsN.
C9H7N.
1-7
2-3
O.I
3-i
o-S
2
4
i-7
3-5
5-i
4.8
5
6.4
13-4
6.7
8.4
30
8-3
SOLUBILITY OF CADMIUM IODIDE IN ANILINE, PYRIDINE AND IN QUINOLINE AT
DIFFERENT TEMPERATURES. (Muchin, 1913.)
Gms. CdI2 per 100 Gms. Sat. Solution in:
t".
40
50
60
70
80
90
100
SOLUBILITY OF CADMIUM IODIDE IN MIXTURES OF SOLVENTS AT DIFFERENT
TEMPERATURES. (Muchin, 1913.)
Composition of Solvent *£*££%? Gms. CdI2 per 100 Gms. Sat. Solution at:
to Mols. Solvent. 'V. 16.8°. 36.8°.
iCH3OH+2CHCl3 ii. 8 ii .o 10.4 9.3
iCHsOH+iCHCla 21.1 22.4 22.3 20.6
iC2H5OH+2CHCl3 16.2 7.5 7.1 6.6
iCjjHsOH+iCHCls 27.8 13.9 14.3 13.6
43.5 25.2 24.1
60.3 34.4
91-5 45-4
i<^H50H+2C6H6 22.8 17.6 16.3(16.3°) 15.2(31.2°)
iC2H50H+iC6H6 37.1 26.1 26.0(15.7°) 26.0 "
aC^OH+iQft 54.1 33.5 35-3(i50)
9.8 6.5
177 CADMIUM IODIDE
SOLUBILITY OF CADMIUM IODIDE IN MIXTURES OF SOLVENTS.
(Muchin, 1913.)
Results for a mixed solvent composed of:
One Mol. Pyridine+One Mol. Chloroform. One Mol. Pyridine-hOne Mol. Benzene.
Cms. CdLz per Gmsi Cdh per . •• Cms. Cdlj per Cms. CHfcper
t°. 100 Gms. t°. 100 Cms. t°. 100 Gms. t°. 100 Gms.
Sat. Sol. Sat. Sol. Sat. Sol. Sat. Sol.
50.1 1.27 63 6.3 57.9 1.77 72.5 32.6
54 1-72 64 8.3 60 2.2 74.0 35.9
56 2.3 64.5 12.35 65 4.2 76 36.3
58 3.0 64 14.8 70 8.1 80 40.8
60 4.0 62 22.0 71 II.5 85 41.6
62 5.6 6I.I5 24.67 71.5 15.0 90.4 42.67
SOLUBILITY OF CADMIUM IODIDE IN ETHYL ETHER CONTAINING WATER AT 12°.
(Tyrer, 19 n.)
Gms. H2O per
100 gms. ether -{-H^O— > o.o o.io 0.30 0.50 0.70 0.90 i.oo i.io 1.14 sat.
Gms. Cdl2 per
100 gms. solvent— > 0.1430.78 2.07 3.36 4.77 6.46 7.30 8.278.68
DISTRIBUTION OF CADMIUM IODIDE AT 30° BETWEEN:
(Dahr and Batter, 1913.)
Water and Amyl Alcohol. Water and Ethyl Ether.
Gms. per 100 cc. c Gms. per 100 cc. c
HaO Layer (c). Alcohol Layer (c1). c/ HzO Layer (c). Ether Layer (c7). c/
47-75 43 I- ii 37 -18 8.38 4.43
29.08 25.86 1.13 30.03 6.61 4.54
14.46 12.55 1.15 15.38 3.09 4.97
10.69 ^.94 1.20 12. 60 2.38 5.29
6-23 4-94 i-33 9-89 1-83 5.40
2.42 i-54 1-55 7-68 i. 06 5.52
i-93 i.io 1.76 4-03 0.73 5.60
1.76 0.94 1.87 3.10 0.51 6.03
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures:
Cadmium Iodide + Cuprous Iodide (Herrmann, 1911.)
+ Mercuric Iodide (Sandonnini, 1914.)
-j- Potassium Iodide (Brand, 1912.)
" + Sodium Iodide
CADMIUM AMMONIUM IODIDES (Mono and Di).
SOLUBILITY OF EACH SEPARATELY IN WATER, ETC.
(Rimbach, 1905; Eder, 1876.)
Cd. Mono Ammonium Iodide. Cd. Diammonium Iodide.
Gms. Cdfc.NHJ per Gms. CdI2.2NHJ per
Solvent. t°. IPO Gms. t«_ too Gms.
Solution. Solvent. Solution. Solvent*
Water 15 52.6 in 14.5 85.97 611.6
Abs. Alcohol 15 53 113 15 59 143
Abs. Ether 15 29.4 41.7 15 10 n
CADMIUM IODIDES 178
CADMIUM POTASSIUM IODIDES, Mono = CdI2.KI.H2O,
Di = CdI2.2KI.2H2O.
CADMIUM DiSODIUM IODIDE CdI2.2NaI.6H2O.
^SOLUBILITY OF EACH SEPARATELY IN WATER, ETC., AT 15°.
(Eder.)
Gms. Gdljj.KI
Solvent.
Water
Abs. Alcohol
Abs. Ether
CADMIUM NITRATE Cd(NO3)2.
SOLUBILITY IN WATER.
(Funk — Wiss. Abh. p. t. Reichanstalt 3 440, 'oo.)
Gms. CdI2.KI
per 100 Gms.
Gms. CdI2.2KI
per 100 Gms.
Gms. CdI2.2NaI
per 100 Gms.
Solution. Solvent.
Solution.
Solvent.
Solution.
Solvent.
51.5 106
57-8
41.7
137
71
53-7
158.8
116.2
...
3-9
4-1
9.0
9-9
Gms. Cd(N03)2
% o. per i oo^ Gms.
Mols. Cd(N03)2 Solid
Solution.
Water.'
per 100 Mols. H2O. Phase.
— 13
37-37
59 -67
4-55
Cd(N03)2.9H20
~ I
47-33
89.86
6.85
Tt
+ I
52-73
in. 5
8.50
11
0
52-37
109.7
8-37
Cd(N03)2.4H20
+ 18
55-9
126.8
9.61
"
30
58-4
140.4
10.7
u
40
61.42
159.2
12. 1
"
59-5
76-54
326.3
25.0
tt
Density of saturated solution at 18° = 1.776.
The eutectic of the system Cd(NO3)2.4H2O + Cd(NO3)2 is at*44.8°and has the
composition Cd(NO3)2.2.65H2O. (Vasilev, 1910.)
CADMIUM OXALATE CdC2O4.3H2O.
i liter of sat. aqueous solution contains 0.033 gm. CdC2O4 at 18°. (Kohlrausch, 1908.)
CADMIUM SILICATE CdSiO3.
Fusion-point data are given for CdSi03 + ZnSiOj. (van Klooster, 1910-11.)
CADMIUM SULPHATE CdSO4.
SOLUBILITY IN WATER.
(Mylius and Funk — W. Abh. p. t. Reichanstalt 3, 444, 'oo; see also Kohnstamm and Cohn — Wied
Ann. 65, 344, '98; Steinwehr — Ann. der Phys. (Drude) [4] 9, 1050, '02; Etard — Ann. chim. phys
[?J 2 536, '94-)
Gms. CdSO4 Gms. CdSO4
t°. per IPO Gms. Ph * °- per 100 Gms. Solid
Solution. Water. Solution. Water.
-17 44.5 80.2 CdSO4>7H2O 40 43.99 78.54 CdSO4.fH2O.
— 10 46.1 85.5 60 44.99 83.68 "
- 5 48.5 94-2 " 73.5 46.6 87.28
-18 43.35 76.52 CdS04.|H20 74.5 46.7 87.62 CdS04.H2O
-10 43.27 76.28 77 42.2 73.02
o 43.01 76.48 85 39.6 65.57
•J-io 43.18 76.00 90 38.7 63.13
20 43-37 76-6o 100 37.8 60.77
For results at high pressures, see Cohen (1909).
179
CADMIUM SULFATE
SOLUBILITY OF CADMIUM SULPHATE IN AQUEOUS SOLUTIONS OP SUL-
PHURIC ACID AT o°.
(Engel — Compt. rend. 104, 507, '87.)
Equivalents per 10 Gms. H2O.
H2S04.
O.
3-87
12.6
28.1
43-3
47.6
53-8
CdS04.
71.6
70.9
62 .4
50.6
40.8
37-o
32-7
23.0
Density
of Solutions.
.609
•591
•545
.476
•435
.421
1.407
1-379
Grams per log Grams H2O.
H2S04.
CdSO4.
O-OO
74.61
1.90
73-87
6.18
65-03
13-78
52-73
21.23
42.52
23-34
38.56
26.38
34-07
35-06
23.96
ioo gms. 95% formic acid dissolve 0.06 gm. CdSO4 at 18.5°. ' (Aschan, 1913.)
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
CdSO4 + Li2SO4, CdS04 + K2SO4 and CdSO4 + Na2SO4 by Calcagni and Marotta
(1913)-
SOLUBILITY OF MIXED CRYSTALS OF CADMIUM SULPHATE AND FERROUS
SULPHATE IN WATER AT 25°.
(Stortenbecker — Z. physik. Chem. 34, 109, 'oo.)
VxUIIlp
usuion 01 ooiu
Gms. per
ioo Gms. H2O.
Mols. per ioo Mols. H2O.
Mol. % Cd.
in Sol.
Crystals of
Solid Phase.
CdSO4.
FeSO4.
Cd.
Fe.
Crystals with a\
} Mols. H2O.
76.02
O-O
6-57
0-0
IOO
IOO
57-6i
10.63
4.98
1.26
79-8
99-o
Crystals with 7
Mols. H2O.
57'6l
10.63
4.98
1.26
79.8
36-6
78.5
34-6
44.6
n. i
. . .
. . .
24.4
4-8
0.0
26.69
o.o
3-I65
o.o
o.o
CADMIUM POTASSIUM SULFATE CdK2(SO4)2
SOLUBILITY IN WATER.
(Wyrouboff, 1901.)
t» G. CdK2(SO4)2 per
ioo Gms. HzO.
16 42.89
31 46.82
40 47-40
Solid Phase.
CdK2(SO4)2.2H20
f o G. CdK2(SO4)2 per
ioo Gms. H2O.
26
31
40
64
Solid Phase.
42.50 CdK2(SO4)2.ijH20
42.80
43-45 ;;
44.90
CADMIUM SODIUM SULFATE 180
CADMIUM SODIUM SULFATE CdNa2(SO4)2.2H2O.
SOLUBILITY IN WATER, ALSO WITH THE ADDITION OF CADMIUM SUL-
PHATE AND OF SODIUM SULPHATE.
(Koppel, Gumpery — Z. physik. Chem. 52, 413, '05.)
Gms. per 100 Gms.
t». Solution.
Gms. per 100 Gms. Mols. per 100 Mols.
H2p- H?O. Solid Phase.
24
30
40
0
10
CdS04.
22.25
22-55
22 .89
40.32
39-91
Na2SO4.
I5-29
I5-65
4-85
5-24
CdSO4.
35-49
36.28
37-24
73-54
72.77
Na2S04.
24.04
24.60
25-45
8.85
9-55
CdSO4. *
3-07 ,
3-!4 ,
3-22 ,
6.36
6.30
5-05]
5.12 [• CdNa2(SO4)2.2H2O
5.28]
•I2}
.21 CdNa2(S04)2.2H20
2O
40
.26
73
.81
9-45
6
•39
.20 I +CdSO4-.|H2O
40
39
.89
7^8
75
•38
13
•56
6
•52
.72
1
• 14.
840
.18
4.60
72
.68
8
•32
6
.29
•05
0
IO
20
37
32
22
•30
•53
.69
6-53
8.69
14.71
66
55
36
•32
•34
•25
ii
14
23
.62
.78
•52
5
4
3
•74
•79
.14 ;
•47
.84
;.98
CdNa2(SO4)2.2H2O
+ Na2SO4.ioH2O
25
16
•33
19.82
25
.60
31
.06
2
.21 3.94^
30
35
40
9
8
9
.21
.26
.98
27.80
29-35
28.27
14
13
16
.62
.26
.24
44
47
46
.14
.06
I
I
I
.26 4.59"
.41 5.86.
CdNa2(SO4)2.2H2O
+ Na2S04
CADMIUM SULFIDE CdS.
1000 cc: H2O dissolves 9 X lo"6 gms. CdS at 18°.
(Weigel, 1906.)
CAESIUM ALUMS
SOLUBILITY OF CAESIUM CHROMIUM ALUM, CAESIUM IRON ALUM,
CAESIUM INDIUM ALUM, AND OF CAESIUM VANADIUM ALUM IN
WATER.
(Locke — Am. Ch. J. 27, 174, '01.)
Formula of Alum.
Cs2Cr2(S04)4.24H20
tt
tt
ii
Cs2Fe2(S04)4.24H20
Cs2In2(S04)4.24H20
Cs2V2(S04)2.24H20
See also Alums, p. 32.
25
30
35
40
25
30
35
40
25
25
Gms. per 100 cc. H2O.
Anhydrous
Salt.
0.96
I .206
I.7I
2.52
3-75
6.04
7-57
0.771
Hydrated
Salt.
1.52
1.91
2-43
2.72
4.01
6.01
9.80
Gram Mols. Salt per
100 cc. H2O.
0.0025
0.0032
O.OO4O5
0.0045
O.OO66
0.0099
0-0156
O.OI72
O-O0204
I8i CAESIUM CHLORAURATE
CAESIUM CHLORAURATE CsAuCl*.
SOLUBILITY IN WATER.
(Rosenbladt, 1886.)
Cms. CsAuCU
Gms. CsAuCU
Gms. CsAuO<
t°.
per 100 Gms.
t°.
per 100 Gms.
t°.
per 100 Gms.
Solution.
Solution.
Solution.
IO
o-5
40
3-2
80
I6.3
20
0.8
50
5-4
90
21.7
30
i-7
60
8.2
IOO
27-5
70
12. 0
CAESIUM FLUOBORIDE CsBFl4.
loo grams water dissolve 0.92 gram CsBFl4 at 20°, and 0.04 gram at 100°.
(Godeffroy, 1876.)
CAESIUM BROMIDE CsBr.
SOLUBILITY OF CAESIUM AND LEAD BROMIDES AND THEIR DOUBLE SALTS
IN WATER AT 25°.
(Foote, 1907.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
1 CsBr^ PbBr2. 7~Cs&- PbBrT^
0.24 0.33 PbBr2+CsPb2Br5 33.65 trace CsPbBr3
0.33 0.36 " " 36-7 " +Cs4PbBr8
1 2. 8s trace CsPb2Br5 46.4 " Cs4PbBr6
a u ti it
17*68 " " +CsPbBr3 54.4 "' " +CsBr
18.58 CsPbBr3 55.23 o CsBr
CAESIUM Mercuric BROMIDE CsBr.2HgBr2.
100 grams saturated aqueous solution contain 0.807 gram CsBr.2HgBr2 at 16°.
(Wells, 1892.)
CAESIUM CARBONATE Cs2CO3.
100 grams absolute alcohol dissolve n.i grams Cs-jCOs at 19°, and 20.1 grams
at b. pt. (Bunsen.)
CAESIUM BiCARBONATE CsHCO3.
100 grams sat. solution in H2O contain 67.8 grams CsHCO3 at about 20°.
(de Forcraud, 1909.)
CAESIUM CHLORATE CsClO3 CAESIUM PerCHLORATE CsClO4.
SOLUBILITY OF EACH IN WATER.
(Calzolari, 1912; see also Carlson, 1910.)
Results for CsClOj. Results for CsClO4.
Gms. CsClOa Gms. CsClOs Gms. CsClOi Gms. CsClO4
t°. per loo Gms. t°. per 100 Gms. t°. per 100 Gms. t°. per 100 Gms.
HzO. H20. HzO. ^ HjO.
o 2.46 50 19.4 o 0.8 50 5.4
10 3.8 60 26.2 10 i.o 60 7.3
20 6.2 70 34.7 20 1.6 7O 9.8
25 7.6 80 45.0 25 2.o(d=I.Ol)8o 14.4(^=1.084)
30 9.5 90 58.0 30 2.6 90 20.5
40 13.8 loo 79.0 40 4.0 zoo 30.0
CAESIUM CHLORIDE 182
CAESIUM CHLORIDE CsCl.
SOLUBILITY IN WATER.
(Berkeley — Trans. Roy. Soc. (Lond.) 203 A, 208, '04; see also Hinrichsen and Sachsel — Z. physik.
Chem. 50, 99, '04- '05; at 25°, Foote.)
t °.
G. CsCl per 100 Gms.
G.Mol.CsCl
0 G. CsCl per ioo Gms.
G. Mol rsri
Solution.
, Water.
per Liter.
v *
Solution
. Water.
per
Liter.
0
6l.7
161
•4
6
•74
60
69.7
229
•7
8
.28
10
63.6
174
•7
7
.11
70
70.6
239
•5
8
.46
20
6S.I
186
•5
7
•38
80
71.4
250
.0
8
.64
30
66.4
197
•3
7
•63
90
72.2
260
.1
8.80
40
67-5
208
.0
7
.86
IOO
73-o
270
.5
8
.96
So
68.6
218
•5
8
.07
119.4
74-4
290
.0
9
y
.22
SOLUBILITY OF MIXTURES OF CAESIUM CHLORIDE AND' MERCURIC CHLORIDE
IN WATER AT 25°. (Foote, 1903.)
Gms. per ioo Gms.
Solution.
Solid Phase.
Gms. per ioo Gms
Solution.
Solid Phase.
CsCl. HgCl2.
65.61 o.o
65.78 0.215
62.36 0.32
CsCl
CsCl + Cs3HgCl6
) Double Salt
CsCl.
17.03
HgCl2.
o.H \
0.42 ,
Double Salt
CsHgCl3= 38.3% CsCl
57.01 0.64
52-35 -23
> CssHgClB
j = 65.1% CsCl
0.61
0.49
2.64
2.91 1
CsHg + CsHg,Cl5
Double Salt
51-08
•44
Cs3HgCl5 + Cs,HgCl4
0.40
3-78 !
CsHg2Cl6 = 23.7% CsCl
49-30
45-95
•49
.69
) Double Salt
\ CsjHgCU = 55.4%CsCl
0.44
0.41
t'el j
CsHgzCl6 + CsHg5Clu
Double Salt
45-23
•73
CsjHgCU + CsHgCl,
0.25
5-65 i
CsHg5Clu= n.i%C6Cl
0.18
7.09
CsH&Clu + HgCl,
o.o
6.90
HgCl2
SOLUBILITY OF MIXTURES OF CAESIUM CHLORIDE AND MERCURIC CHLORIDE IN
ACETONE AT 25°. (Foote, 1911.)
Gms. per ioo Gms. Solution.
. pfpi -7T-F1 ' Solid Phase-
CsCl. HgCh.
0.48 28.48 CsC1.2HgCl2
0.48 39.65 "
0.47 44.40 " +CsCl.5HgCl2
0.32 49.83 CsC1.5HgCl2
Gms. per ioo Gms. Solution
CsCl. ' HgClz.
O
O.O2
O.l6
0.032
O.II
0.19
0.25
0.45
0.46
0.56
Solid Phase.
CsCl
Mixed salts
0.17
13.08 CsCl.HgCl2
21 .50
0.20 57.74
0-13 57-76 " +HgCl2
57.74HgCl2
27.2 " + CsCl.2HgCl2 o.o
CAESIUM Iridium CHLORIDES Cs2IrCl6, etc.
loogms. HzO dissolve o.oi I gm. caesium chloroiridate, Cs2lrCleat 19°. (Delepine, 1908.)
ioo ' 0.05 gm. caesium hexachloroiridite, Cs3IrCl6.3H2O at 19°.
ioo " 0.83 " caesiumaquopentachloroiridite,|Cs2H2OIrCl6ati90.
CAESIUM Platinic CHLORIDE CsPtCle.
IOO gms. H2O dissolve 0.135 Sm- CsPtCle at 2O°. (Rosenheimand Weinheber, 1910-11.)
CAESIUM Tellurium CHLORIDE CsTeCl6.
SOLUBILITY IN AQUEOUS HYDROCHLORIC ACID. (Wheeler, 1893.)
ioo parts HC1 (Sp. Gr. 1.2) dissolve 0.05 part CsTeCU at 22°.
ioo parts HC1 (Sp. Gr. 1.05) dissolve 0.78 part CsTeCle at 22°.
CAESIUM Thallium CHLORIDE 3CsCl.TlCl3.2H2O.
ioo parts H2O dissolve 2.76 parts 3CsCl.TlCl3.2H2O at 17°, and 33.3 parts at
I OO°. (Godeffroy, 1886.)
183
CAESIUM CHLORIDE
Freezing-point lowering data (solubilities, see footnote, p. i) are given for the
following mixtures of caesium chloride and other salts.
Mixture. Authority.
Caesium Chloride + Cuprous Chloride (Sandonnini and Scarpa, 1912; Sandonnini, 1914.)
-j- Silver Chloride
+ Thallium Chloride " "
+ Lithium Chloride (Korreng, 1915; Richards and Meldrum, 1917.)
+ NaCl (Richards and Meldrum, 1917.)
-|-v Potassium Chloride (Zemcznzny and Rambach, 1910.)
+ Rubidium " "
+ Sodium
CAESIUM CHROMATES, Cs2CrO4, Cs2Cr2O7, etc.
SOLUBILITY IN WATER AT 30°.
(Schreinemakers and Meijeringh, 1908.)
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
Gms. per 100 Gms. Sat.
Sol.
Solid Phase.
CsaO.
70.63
69.22
36.06
31.00
31.68
35-80
3I-05
24.05
3-°4
1.61
1.18
0.586
CrOs.
0.0
O.II9
1.883
7-523
9.652
13.08
10.79
8.98
2.16
4-57
7-95
15-05
' CS20.
CrOs.
0.169
21 .21
t 0.096
25-59
1.89
36.19
2.79
41.68
3.29
44-23
±3.13
±44-45
2.96
44.66
3-40
46.03
3-94
56.77
>10 4.35
62.70
2.33
62.50
0
62.28
" +082014013
" +Cr03
CrO3
CAESIUM FLUORIDE CsF.i|H2O.
100 gms. H2O dissolve 366.5 gins. CsF at 18°, solid phase CsF.i£H2O.
(de Forcrand, 191 x.)
CAESIUM HYDROXIDE CsOH.
100 gms. sat. solution in H2O contain 79.41 gms. CsOH at 15° (de Forcrand,
i9Oo,a); for 30°, see above.
CAESIUM IODATE CsIO4.
loo parts H2O dissolve 2.6 parts CsIO3 at 24°, and 2.5 parts 2CsIO3.I2O6 at
21°. (Wheeler, 1892; Barker, 1908.)
CAESIUM Per IODATE CsIO4.
loogms. H2O dissolve 2. 15 gms. CsIO4at 15°,
CAESIUM IODIDES Csl, CsI3, etc.
sat. solution = 1 .0166. (Barker, 1908.)
SOLUBILITY IN WATER AT 25°.
(Foote and Chalker, 1908.)
Gms. per 100 Gms. Sat. Solution. Empirical Comp.
Csl.
7.72
7.69
i.
1.19
2.40
1.23
2-35
1.23
2-39
1-25
of Residue
CsI3.29
CsI3.98
Csi5:75
CsI7.43
CsIiQ.3
Present in Residue.
CsI3 and
it «
CsI5 and I
u u
CAESIUM IODIDE
184
CAESIUM IODIDE Csl.
SOLUBILITY OF MIXTURES OF CAESIUM IODIDE AND IODINE IN WATER.
(Foote — Am. Ch. J. 29, 210, '03.)
Gms. per ioo Gms.
t °. Solution. 40
Gms. per ioo Gms.
Solution.
Solid Phase at
Csl.
i.
Csl.
i.
both Temps.
-4
27.68
o.o
35-6
51.48
o.o
Csl
-4
27.52
0.09
35-6
51.66
0.71
Csl and CsI3
-4
3.18
0.31
35-6
10.72
1.78
CsI3 and CsI5
— 0.2
0.85
o.34
35-6
3-74
i. 60
CsI5 and I
Gms. per ioo Gms.
t <\ Solution.
Csl.
i.
52.2
16.75
4-52
52.2
6.69
3-36
52.2
6.72
3-32
52.2
6.65
3-45
73
26.98
15-07
73
16.66
10.50
73
6.27
4-08
In Separated Heavy Solution
Gms. per ioo Gms. Solution.
Csl.
I.
.rnase.
CsI3 and CsI5
CsI5 and I
22.94
73-72
CsI5
22.8o
I
CsI3 and CsI6
27.56
68.40
CsI5
17.68
80.02
I
CAESIUM (Tri) IODIDE CsI3.
100 cc. saturated aqueous caesium iodide (about 17 per cent Csl)
solution contain 0.97 gram CsI3 at 20°, density of solution =1.154.
(Wells — Am. J. Sci. [3] 44, 221, 'pa.)
CAESIUM NITRATE CsNO3.
SOLUBILITY IN WATER.
(Berkeley — Trans. Roy. Soc. (Lond ) 203 A, 213, '04.)
Gms. CsNO3 per
t °. ioo Gms.
G. Mols.
CsNO3 t °.
Gms. CsNO3 per
ioo Gms.
G. Mols CsN03
Solution.
Water.
per
Liter.
Solution.
Water'.
per Liter.
0*
8-54
9
•33
o.
476
60
45-6
83
.8
3
.41
10
12-97
14
•9
o.
725
70
51 .7
107
.0
4
.10
2O
I8.7
23
.0
I.
II
80
57-3
134
.0
4
.81
30
25-3
33
•9
I .
58
90
62 .0
I63
.0
5
-50
40
32.1
47
.2
2.
12
IOO
66.3
197
.0
6
.19
50
39-2
64
•4
2.
73
106
.2 68.8
2 2O
•3
6
•58
THE ICE CURVES FOR MIXTURES OF CAESIUM NITRATE AND WATER,
DETERMINED BY THE SYNTHETIC METHOD.
(Jones, 1908.)
Solubility curve.
t° of Crystalli- Gms. CsNOs per
zation. ioo Gms. HjO.
-0.3 0.21
— 0.4 1.28
— 1.2 6.01
— i.l 8.0
Solid
Phase.
Ice
M
u
Supersolubility curve.
t8 of Crystalli- Gms. CsNOs per Solid
e'zation. ioo Gms. HjsO. Phase.
Ice
— 1.2
-2-5
-3-2
-3.2
O.2I
1.28
3-99
6.01
8
-i.4(Eutec.)
The eutectic is given as —1.254° and 8.51 gms. CsNOs per ioo gms. H2O, by
Washburn and Maclnnes (1911).
185
CAESIUM "OXALATE
CAESIUM OXALATE Cs2C2O4.H2O.
SOLUBILITY OF MIXTURES OF CAESIUM OXALATE AND OXALIC ACID IN WATER
AT 25°.
(Foote and Andrew, 1905.)
Varying amounts of the two substances were, dissolved in hot water and the
solutions allowed to cool in a thermostat held at 25°.
Gms. per 100
Gms. Solution.
G. Mols. per 100
G. Mols. H20.
Solid
Phao»
HjC^. CsjjCjA. H2C2O4. Cs2C2O4.
i na.se.
10
.20
2.274
H2C2O4.2H2O
10
.29
o
.61 2.314
0
•035
H2C204.2H20+H3Cs(C2O4)2.2H20
7
.90
9
.92 1.924
o
.614 ^
Double Salt.
4
.11
25
.12 I.l62
I
.81
J
H3Cs(C2O4)2.2H2O
4
•32
27
•55
•279
2
.06
H3Cs(C204)22H20+H4Cs2(C204)3
4
.27
28
.30 ]
.267
2
.14
I
Double Salt.
4
• 40
35
.90 3
.476
3
.07
\
H4Cs2(C204)3
4
.82
40
.10
•752
3
.71
H4Cs2(C204)3+HCsC204
4
3
i
•45
•05
.04
42
48
68
.32 ]
.80
.69 c
.672
.268
5.688
4
5
ii
•05
.16
•56
\
Double Salt.
HCsC204
0
.91
71
.24 0.648
13
.06
HCsC2O4+ HgCsg^OJ-
o
•77
73
•45 <
3.598
14
•51
I
Double Salt.
0
•75
74
.04 0.596
14
.96
\
H6Cs8(C204)7
o
•74
75
.20 0.625
15
•93
H6Cs8(C204)7+ Cs2C204.H20
o
.0
75
.82 o.o 15
•97
Cs2C204.H20
CAESIUM Telluracid OXALATE Cs2[H6TeO6.C2O4].
100 gms. H2O dissolve 6.42 gms. Cs2[H6TeO6.C2O4] at o°, 12.39 S1118- at 20°,
15.08 gms. at 30°, 19.78 gms. at 40° and 27.66 gms. at 50°.
(Rosenheim and Weinheber, 1910-11.)
CAESIUM PERMANGANATE CsMnO4.
100 cc. sat. aqueous solution contain 0.097 gm. CsMnO4 at i°, 0.23
gm. at 19°, and 1.25 gms. at 59°. (Patterson — J. Am. Chem. Soc. 28, 1735, '06.)
CAESIUM SELENATE Cs2SeO4.
100 grams H2O dissolve 245 grams Cs2SeO4 at 12°.
(Tutton — J. Chem. Soc. 7ii 850, *97<)
CAESIUM SULPHATE Cs2SO4.
SOLUBILITY IN WATER.
(Berkeley — Trans. Roy. Soc. (Lond.) 203 A, 210, '04.)
Gms. Cs2SO4 per
tc. ioo Gms.
G. Mols.
Cs2S04 t°.
Gms. Cs2SO4 per
ioo Gms.
G.Mols.
Cs2S04
Solution.
Water.
per
Liter.
Solution.
Water.
per Liter.
O
62
.6
I67
.1
3
• 42
60
66.7
199
•9
3-78
10
63
•4
173
.1
3
.49
70
67.2
205
• O
20
64
.1
I78
•7
3
•56
80
67.8
210
•3
3-88
30
64
.8
184
.i
3
.62
90
68.3
214
•9
3-92
40
65
•5
I89
9
3
.68
IOO
68.8
220
•3
3-97
50
66
.1
194
9
3
•73
108.6
69.2
224
•5
4-00
CAESIUM DOUBLE SULFATES 186
SOLUBILITY OF CAESIUM DOUBLE SULPHATES IN WATER AT 25°.
(Locke — Am. Ch. J. 27, 459, 'ox.)
Cms. Anhydrous Salt Gm. Mols.
Name. Formula. per 100 Cms. Salt per 100
Solution. Water. Gms.H2O.
Caesium Cadmium Sulphate - Cs2Cd(so4)2.6H2o 58.16 139.9 0.2455
Caesium Cobalt Sulphate Cs2Co(so4)2.6H2o 29.52 41.9 0.081
Caesium Copper Sulphate c^Cu(so4)2.6H2o 31-49 46.0 0.0882
Caesium Iron Sulphate Cs2Fe(so4)2.6H2o 50.29 101.1 0.1967
Caesium Magnesium Sulphate Cs2Mg(so4)2.6H2o 34-77 53-3 o . i 106
Caesium Manganese Sulphate Cs2Mn(SO4)2.6H2o 44 .58 80. 4 0.157
Caesium Nickel Sulphate Cs2Ni(so4)2.6H2o 20.37 25-6 0.0495
Caesium Zinc Sulphate Cs2Zn(so4)2.6H2o 27.87 38.6 0.0738
SOLUBILITY OF CAESIUM SODIUM SULFATES IN WATER AT 25°.
(Foote, 1911.)
Cms, per 100 Cms. Sat. Solution. Per cent CsSC>4 Empirical C9mposition of
Cs2SO4. NazSO4. in Residue. **, * Residue.
54.65 11.44 89.98 iNa2SO4.3.53Cs2SO4
54.58 11.63 78.22 iNa2S04.i.4iCs2SO4
54.81 11.25 34.67 4.8Na2SO4.iCs2SO4
The author's solubility method for determination of the formation and com-
position of double salts is described in the paper containing the above results.
CAESIUM DihydroxyTARTRATE Cs2C4H4O8.2H2O.
100 gms. H2O dissolve 22.5 gms. Cs2C4H4O8.2H2O at o°. (Fenton, 1898.)
CAFFEINE C6H(CH3)3N4O2.H2O.
SOLUBILITY IN WATER.
(Average curve from results of Zalai, 1910; Pellini, 1910, and U.S.P., 8th Ed.)
t» Gms. C6H(CH3)3N4O» t» Gms. C6H(CH3)3N4O»
per 100 Gms. HiO. per 100 Gms. HjO.
o 0.6 40 . 4.64
15 i.o 50 6.75
20 1.46 60 9.7
2$ 2.13 70 13.5
30 2.8 80 19-23
SOLUBILITY OF CAFFEINE IN ORGANIC SOLVENTS.
Solvent t° Gms- C5H(CH3)3N402 Solve_t t» Gms. CsH(CHs)iN4O,
bolvent. t . pe,. I00 Gms- Solvent. bolvent. t . per IQQ Gmg Solvent.
Ethyl Alcohol 25 1.32(2) Carbon Tetra- ( 18 0.09(4)
" " 25 1.88(1) chloride ] 20 0.26(6)
60 5.85(1) 'b.pt. 0.70(4) .
Methyl ' 25 1.14(2) Chloroform 17 12.9 (5)
Amyl " 25 o.5o(3)(<*»=o.8io) 25 12.3 (i)
Amyl Acetate 30.5 0.72(3)0*30=0.862) 25 11.92(2)
Acetic Acid (99.5%) 2 1. 5 2.6 (3) b.pt. 15.63 (4)
Acetone 30.5 2 . 3 2 (3) (dm =0.83 2) Ether 1 8 o . 1 2 (4)
Aniline 30.5 29.4(3)0*30=1.080) 25 0.27(1)
Benzaldehyde 30.5 13.1(3)0*30=1.087) " b.pt. 0.30(4)
Benzene 18.0 0.91(4) Trichlorethylene 15 0.76(7)
25.0 1.16(2) Dichlorethylene 15 1.82(7)
30. 5 i . 23 (3)0*30=0.875) Pyriclme " 20-25 34.39 (8)
b.pt. 5.29(4) 50% Aq. Pyridine " 11.12(8)
Carbon Bisulfide 17 0.06(5) Toluene 25 0.58(3)^=0.861)
Xylene 32.5 1.13(3)0*32=0.847)
(i) = U. S. P.; (2) = Schaefer, 1913; (3) = Seidell, 1907; (4) = Gockel, 1898; (5) = Commaille, 1875;
(6) = Gori, 1913; (7) = Wester and Bruins (1914); (8) = Dehn, 1917.
Data for the solubility of caffeine in mixtures of alcohol and chloroform and
alcohol and benzene are given by Schaefer (1913).
187
CAFFEINE
SOLUBILITY OF CAFFEINE IN AQUEOUS SOLUTIONS OF SODIUM BENZOATE AND
VICE VERSA. (Peilmi, 1910.)
Results at 25°.
Gms. per too Gms. HzO.
C8H10N402.
CrHiOiNa.
2.13
O
8.32
6.67
38.10
45
5*-74
76.75
46.27
76.68
24.79
69.56
9-47
62.97
o
61.17
Solid Phase.
Results at 40°.
Gms. per too Gms. H2O.
+C7Hfi02Na.H20
4°- 64
o
3J-43
25-3I
56.82
69.68
57-99
74.64
55.98
74.02
18.31
67.97
0
59.82
Solid Phase.
SOLUBILITY OF CAFFEINE IN AQUEOUS SOLUTIONS OF SODIUM SALICYLATE AND
VICE VERSA. (P^llini and Amadori, 1912.)
Results at 25° . Results at 40°.
Gms. per 100 Gms. H2O.
C8H10N402.
2.13
38.36
CrtUOsNa.
0
30.76
55-23
74-32
16.78
47-31
68.81
124.96
13.22
121 .27
9-03
120.54
0
115-43
Solid Phase.
CsH10N402.H20
Gms. per 100 Gms. H2O.
:8H10N402.
CvHsOsNa.
4.64
O
59-49
37-47
86.49
62.47
95-94
69.15
26.93
131-52
iQ-75
124-35
0
119.66
Solid Phase. •
Data for the depression of the freezing-point of sodium salicylate solutions by
caffeine and theobromine are also given.
DISTRIBUTION OF CAFFEINE BETWEEN WATER AND CHLOROFORM. (Marden, 1914.)
Grams Caffeine in:
105 cc. EbO Layer.
o . 0090
O.OlSo
0.0291
50 cc. CHCla Layer.
0.0563
o . 1048
0.1770
Ratio of Caffeine in
Equal Vols. H2O and CHC1«.
0.0456
o . 0492
O.0470
Gms. Ca(CH3COO)2
. per 100 Gms.
CALCIUM ACETATE Ca(CH3COO)2.2H3O.
SOLUBILITY IN WATER. (Lumsden, 1902; Krasnicki, 1887.)
Gms. CaCCHaCOCOa
jo^ per IPO Gms. Solid Phase.
Water.
37.4 Ca(CH3COO)2.2H2O
Ca(CH3COO)2.2H2O
Ca(CH3COO)2.2H2O
Ca(CH3COO)2.2H2O
Ca(CH3COO)2.2H2O
Ca(CH3COO)2.2H2O
Solid Phase.
30
40
32-9
31-1
Solution.
o 27.2
10 26.5 36.0
20 25.8
25 25.5
25-3
24-9
SOLUBILITY OF CALCIUM ACETATE IN AN AQUEOUS SATURATED SOLUTION OF
SUGAR AT 31.25°. (Kohier, 1897.)
100 gms. solution contain 8.29 gms. Ca(CH3COO)2 + 60.12 gms. sugar.
100 gms. water dissolve 26.3 gms. Ca(CH3COO)2 + 190.3 gms. sugar.
loo cc. anhydrous hydrazine dissolve i gm. calcium acetate at room temp.
(Welsh and Broderson, 1915.)
34-7
34-2
33-8
33-2
60
80
84
85
90
IOO
Solution.
24.6
25-1
25-3
24-7
23-7
22-9
Water.
32.7 Ca(CH3COO)2.2H20
33.5 Ca(CH3COO)2.2H20
33.8 Ca(CH3COO)2.2H20
Ca(CH3COO)3.H2O
Ca(CH3COO)2.H2O
29 . 7 Ca(CH3COO)2.H,O
CALCIUM ACETATES
188
CALCIUM (Tri) Methyl ACETATE Ca[(CH3)3CCOO]2.
CALCIUM (Di) Ethyl ACETATE Ca[(C2H6)2CHCOO]2.
CALCIUM Methyl Ethyl ACETATE Ca[CH3(C2H6).CHCOO]2.
SOLUBILITY OF EACH IN WATER.
(Landau — Monatsh. Chem. 14, 717, '93; Keppish — Ibid, g, 600, '88; Sedlitzki — Hid. 8, 573, '87.)
Ca. Tri Methyl Acetate. Ca. Di Ethyl Acetate. Ca. Methyl Ethyl.
Acetate.
Gms. Ca(CsH9O2)2
t o. per 100 Gms.
Water. Solution".
0
7 .30
6.81
10
6.84
6.40
20
6-54
6.14
30
6.40
6.01
40
6.44
6.05
50
6.64
6.22
60
6.86
6.42
70
7.11
6.64
80
7-38
6.87
Gms. '
Ca(CeHiiO2)2
Gms. Ca(C5H902)2
per
100 Gms.
per ipo Gms.
'Water
. Solution.
Water. Solution.
30-3
23.22
28.78 22-35
27.8
2i-75
31.71 24.07
25.6
20.38
33 -76 25.23
23-7
19.16
34.92 25.89
22 .1
18.10
35.20 26.04
20.8
17.22
34.60 25.71
19.9
16.60
33.11 24.89
19.2
i6.n
30.74 23.41
27.49 21.56
CALCIUM Methyl Propyl ACETATE Ca[CH3(C3H7).CHCOO]L.
CALCIUM (Di) Propyl ACETATE Ca[(C3H7)2CHCOO]2.
CALCIUM (Iso) Butyl ACETATE Ca[(CHE)2CH(CH2)2COO]2.
SOLUBILITY OF EACH IN WATER.
(Stiassny — Monatsh. Chem. 12, 596, '91; Furth — Ibid. 9, 313, '88; Konig — Ibid. 15, 22, '94.)
Ca. Methyl Propyl Acetate. Ca. Di Propyl Acetate. Ca. Iso Butyl
Acetate.
Gms. Ca(C6HnO2)2
t o. per 100 Gms.
Water.
Solution.
O
16.58
14.22
10
15.80
I3-65
2O
15.14
13.15
30
I4.6l
"•75
40
14.21
12.45
50
13-94
12.24
60
13-79
12.13
70
I3-78
12.12
80
13.89
12. 2O
90
Gms. Ca(C8H15O2)2
per 100 Gms.
Gms. Ca(C6H11O2)2
per TOO Gms.
Water.
Solution.
Water.
Solution.
9
•57
8
•73
7
.48
6
.96
8
•35
7
•7i
6
•38
5
•99
7
.19
6
•7i
5
.66
5
•36
6
.11
5
•77
5
•3i
5
.04
5
.09
4
.84
5
•3i
5
.04
4
.14
3
98
•5
.68
5
•37
3
•25
3
15
6
.41
6
.02
2
•44
2
38
7
•51
6
.98
I
•65
I.
62
8
•97
8
•23
.
10
•79
9
•74
CALCIUM BENZOATE Ca(C6H5COO)2.
loocc. sat. solution in water contain 3.02 gms. Ca[C6H6COO]2at 26°. (de Jong, 1912.)
100 gms. sat. solution in water contain 8.6 gms. Ca[C6H5COO]2 at 15° and 10.2
gms. at I OO°. (Tarugi and Checchi, 1901.)
CALCIUM BORATES CaB2O4.4H2O, CaB2O4.6H2O.
SOLUBILITY OF EACH SEPARATELY IN WATER.
(Mandelbaum, 1909.)
3O
50
70
90
0.0365
0.036
0.048
0.0315
0.310
0.307
0.392
0.310
(amorphous)
B203.
30 0.0205
50 0.032
70 0.068
90 0.0675
0.254
0-353
0-457
0-359
CaB204.6H2O
" (cryst.)
I89
CALCIUM BORATE
SOLUBILITY OF CALCIUM BORAXES IN AQUEOUS SOLUTIONS OF BORIC, Aero
AT 30°.
(Sborgi, 1913-)
Gms. per 100 Gms. Sat
.Sol.
Solid
Gms. per 10
o Gms. Sal
:. Sol.
Solid
'BzOs.
CaO.
Phase.
BijOa. CaO.
Phase.
0
.014
O.
126
Ca(OH)j
0.
869
0.
067
2.3.9
0
.032
0.
140
"
I.
116
0.
076
•
0
.098
0.
194
"
I.
339
0.093
" +1.3.12
O
.127
O.
217
" +1.1.6
2.
058
0.
093
1.3.12
0
•134
0.
220
1. 1. 6
2.
509
o.
099
"
0
.138
O.
118
H
2.
730
0.
III
"
O
.162
O.
106
"
3-
732
0.
325
(C
O
.166
0.
107
" +2.3-9
2.
798
0.
109
M
0
.171
O.
109
" "
3-
313
0.
143
"
O
.290
0.
052
2-3-9
3-
841
o.
152
It
0
.610
0.
054
"
4-
250
0.
155
" +HiBO,
0
.767
o.
059
"
4-
179
o.
137
HaBOj
1. 1.6 =
CaO,
,B2O3.6H2O,
2.3-9
= 2Ca0.3B2O8.9H2O,
I-3-
12 = CaO.3B203.i2H2O.
Many determinations, in addition to
the above, are
given in the original paper.
CALCIUM BROMIDE
CaBr2.6H2O.
SOLUBILITY IN WATER.
(Kremers, 1858; ' Etard,ri894, gives results which yield an irregular curve and are evidently less
than those of Kremers.)
Solid Phase.
CaBn.6HjO +CaBr».4HjO
CaBr,.4H,0
* Eutec. t tr. pt.
Density of saturated solution at 20° = 1.82.
Data for the system calcium bromide, calcium oxide and water at 25° are given
by Milikau (1916).
Freezing-point data are given for mixtures of calcium bromide and calcium
chloride, calcium bromide and calcium fluoride by Ruff and Plato, 1903.
t°. -
-22*
0
10
20
25
Gms. CaBrz per
100 Gms.
Solid Phase.
CaBtt.SHzO+Ice
CaBr2.6H2O
<(
it
t°.
34-
40
60
80
105
Gms. CaBra per
100 Gms.
Water. Solution.
ioi 50.5
125 55-5
132 57
143 58.8
153 60.5
Water. Solution.
2f 185 65.1
213 68.1
278 73-5
295 74-7
312 75.7
CALCIUM PerBROMIDE CaBr4.
Data for the formation of calcium perbromide in aqueous solutions at 25°
are given by Herz and Bulla (1911). The experiments were made by adding
bromine to aqueous solutions of CaBr2 and agitating with carbon tetrachloride.
From the bromine content of the CC14 layer, the amount of free bromine in the
aqueous layer can be calculated on the basis of the distribution ratio of bromine
between water and CC14. This furnishes the necessary data for calculating the
amount of ^calcium perbromide existing in the aqueous layer.
CALCIUM BUTYRATB 190
CALCIUM (Normal) BUTYBATE Ca[CH3(CH2)2COO]2.H2O.
CALCIUM (Iso) BUTYRATE Ca[(CH3)2CH.COO]2.5H2O.
SOLUBILITY OF EACH IN WATER.
(Lumsden — J. Chem. Soc. 81, 355, '02; see also Chancel and Parmentier — Compt. rend. 104, 474,
'87; Deszathy — Monatsh. Chem. 14, 251, '93, and also Hecht — Liebig's Annalen 213, 72, '82, give
results for the normal salt which are somewhat below those of Lumsden for the lower temperatures.
SedJitzki — Monatsh. Chem. 8, 566, '87, gives slightly different results for the iso salt.)
Calcium Normal Butyrate. Calcium Iso Butyrate.
Gms. Ca(C4H7O2)2 Cms. Ca
t o^ per iqo Gms. t °. per 100 Gms.
Water. Solution. Water. Solution.
o 20.31 16.89 o 20.10 16.78 Ca(C4H7O2)2.5H2O
10 19-15 16.08 20 22.40 18.30-
20 18.20 15.39 30 23.80 19.23
25 I7-72 I5-°5 4° 25.28 20.65
30 I7-25 14-71 60 28.40 22.12
40 16.40 14.09 62 28.70 22.30
60 15.15 13.16 65 28.25 22.03 Ca(C4H703)2.H2O
80 14-95 I3-°I 80 27.00 21.26
100 I5-^5 I3-^9 Io° 26.10 20.69
CALCIUM d CAMPHORATE Ci0H14O4Ca.7H2O.
SOLUBILITY OF CALCIUM CAMPHORATE IN AQUEOUS SOLUTIONS OF CAMPHORIC
ACID AT 15° AND VICE VERSA.
(Jungfleisch and Landrieu, 1914.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
Sohd Phase' ' ' Sohd Phase.
C^^Ca.
1.35 1.23 C8HH(COOH)8 2.90 7.75 C8H14(COOH)2
1-57 1.97 " 3 8.66 " +C10Hi4O4.Ca.7H2O
I.7I 2.55 " 3.07 8.57
2.18 4.34 « 1.50 7.94
2-33 4-73 " o 7.37
gms. CioHuC^Ca per 100 gms. sat. solution.
CALCIUM CAPROATE (Hexoate) Ca[CH3(CH2)4COO]2.H2O.
CALCIUM 3 Methyl PENTANATE Ca[CH,.CH2.CH(CH,)CH2.COO]2.3H2O.
CALCIUM CAPRYLATE Ca[CH3(CH2)6COO]2.H2O.
SOLUBILITY OF EACH IN WATER.
(Lumsden; the Pentanate, Kulish, 1893; see also Keppish, 1888, and Altschul, 1896,
for results on the Caproate.)
Ca. Caproate. Ca. 3 Methyl Pentanate. Ca. Caprylate.
Gms. CaCCeHnO^j per
Gms.Ca(C6HnO2)2l
>er 100 Gms
• Gms. Ca(C8Hi5O2)2 ]
'
loo Gms. H20.
" Water.
Solution.
loo Gms. HzO.
0
2.23
12-33
10.98
o-33
20
2.18
I7.I8
14.66
0.31
40
2.15
18.99
15-97
0.28
50
2.IO
18.73
I5-78
0.26
60
2-15
17.71
15.04
0.24
80
2.30
13-37
II.80
0.32
100
2-57
9-94
9.04
0.50
CALCIUM CARBONATE
CALCIUM CARBONATE CaCO3.
EQUILIBRIUM IN THE SYSTEM CaO-H2O-CO2 AT 16°.
The following data for the solubility of calcite (CaCO3) in water at 16° in con-
tact with air containing the partial pressure P of CO2 were calculated from the
results of Schloesing (1872), Engel (1888), and others by Johnston (1915) and
Johnston and Williamson (1916). These authors describe the changes in the
system resulting from a gradual increase in partial pressure of COa, as follows:
"We begin by considering the equilibrium between the hydroxide M(OH)2 and the aqueous
solution saturated with it as affected by a progressive increase from zero of the partial pressure
P of CO2 in the atmosphere in contact with the solution. Addition of CCk is followed by a dis-
tribution between the vapor and liquid phases until there is equilibrium between the residual
partial pressure of CQj and the HzCOs in solution, and in ^urn between the latter and the
several ions; the net effect of this is a definite decrease in [OH ], the concentration of hydroxide
ion, which necessitates that more of the hydroxide dissolve in order to keep the solubility-
product [M++][OH ]2 constant. Consequently the total concentration of M++ increases,
part of it being now associated with carbonate and bicarbonate; in other words, the apparent
solubility of the base increases if the method of analysis of the solution is a determination of
M, whereas it would decrease if one should determine [OH ]2. This process continues until
the product [M++][CO3=] reaches the value requisite for the precipitation of MCOs (on the
assumption that supersaturation does not occur) which, for a given base, takes place at a
definite value of P which depends only upon the temperature; this transition pressure Pi is,
at a given temperature, the highest under which solid hydroxide is stable and the lowest at
which solid carbonate is stable.
At Pi the solubility (as measured by the total [M]) begins to diminish, because increase of
P increases [CO3=] while the product [M-H-][CO3=] must remain constant so long as MCO3 is
the stable solid phase; this increase of [CO3=] continues until a definite pressure Po is reached,
when the formation of bicarbonate in the solution becomes the predominant reaction and
[CO3=] begins to decrease again. JP0 is thus a minimum in the solubility curve. With
further increase beyond Po the concentration of both M-H- and HCOs increases steadily
until the precipitation value of the product [M-H-][HCOs~]2 is reached at Pz, which is a transi-
tion pressure at which both carbonate and bicarbonate are present as stable solid phases.
Beyond P2 bicarbonate alone is stable, and its total solubility falls off very slowly with
further increase of partial pressure of CCh."
THE CALCULATED ION-CONCENTRATIONS AND SOLUBILITY OF CALCITE IN
WATER AT 16° IN CONTACT WITH AIR CONTAINING THE PARTIAL PRESSURE
P OF CO2.
Partial Pressure P
of CO2 Measured
in Atmospheres.
Ion-concentrations per Liter X 10-*.
Total Ca,
Mols. per
* Liter
Xio-*.
Grams
CaCOa per
Liter.
Ca-H-.
OH-.
C0s=.
HCOr.
3
.16X10-"
138
•5
277
O.OO7I
o
.0000235
2
2
.80 Xio-10
6
.81
13
-3
0.144
0
.01
.
. .
0.074
9
.78Xio-9
2
•377
3
.82
0.414
0
.10
0.026
6
.i4Xio~8
I
•654
i
.82
0-593
o
•30
.
O.OlS
2
.19X10-7
I
.476
i
.02
0.665
0
.60
.
0.016
3
.73X10-7
I
•459
o
.787
0.672
o
.787
.
0.0159
3
.85X10-7
I
•459
o
•774
0.672
o
.80
.
. .
0.0159
6
.07X10-7
I
•473
0
.614
0.666
i
.
. .
0.016
7
.62 Xio"6
2
•051
0
.147
0.478
3
.
0.022
7
.63X io~5
3
•777
0
•034
0.260
7
.
0.040
2
.I5X lo"4
5
.197
0
•0174
0.188
10
.
. .
0.056
2
Xio"4
5
.09
o
.0182
0.19
9
.96
5
•52
0.055
2
•5 Xio-4
5
.46
o
•oi57
0.18
10
•54
5
•93
0.059
3
Xio-4
5
•79
0
.0140
0.17
ii
.22
6
.31
0.063
3
•5 Xio-4
6
.08
0
.0126
0.16
ii
.82
6
•64
0.066
4
XlO"4
6
•35
o
.0115
0.16
12
.36
6
•94
0.069
4
.5 Xio"4
6
•59
o
.0107
0.15
12
.86
7
.21
0.072
5
Xio-4
6
.82
o
.0100
0.14
13
•32
7
.46
0.075
CALCIUM CARBONATE
192
THE SOLUBILITY OF CALCIUM CARBONATE (CALCITE) IN WATER AT 16° IN
CONTACT WITH AIR CONTAINING PARTIAL PRESSURE P OF CO2.
(Calc. from Schloesing, 1872, and Engel, 1888, by Johnston, 1915.)
Total Ca, Mols. Total Ca(HCp3)j
per Liter. Mols. per Liter
0.007825 0.007874
0.008855 0.008854
O.OO972
O.OIO86
0.01085
O.OI4II
0.01834
P of CO2 in
Atmospheres.
Total (Ja, Mols.
per Liter.
Total ua(.nuj3)2
Mols. per Liter.
P of CCh in
Atmospheres.
o . 000504
o . 000746
0.000731
0.4167
0.000808
O.OOO85O
0.000837
0-5533
0.00333
0.001372
0.001364
0.7297
0.01387
0.002<23I
O.OO2226
0.9841
O.O282O
0.002965
O.O0296I
i
o . 05008
0.003600
0.003597
2
0.1422
0.005330
0.005328
4
0.2538
o . 006634
0.006632
6
0.02139
O.OO972
O.OIO86
0.01085
O.OI4II
0.01834
0.02139
THE SOLUBILITY OF CALCIUM CARBONATE] (CALCITE) IN WATER AT 25° IN
CONTACT WITH CO2 UNDER INCREASING PRESSURES. (McCoy and Smith, 1911.)
B* Cot C^vl
Solid Phase.
CaC03
tt
Appro*. Pres-
sure of CO2 in
Mols. per Liter Sat. Solution.
Gms. per Liter Sat. Sol.
Atmospheres.*
H2COs.
Ca(HCO3)2.
H2COs.
Ca(HCOs)2.
O.I
0.003522
0.004Il6
0.22
0.67
I.I
0.03728
0.009734
2-3
I.58
9.9
0.3329
0.02236
20. 6
3.62
13.2
0.444
0.02495
27-5
4.04
16.3
0.550
0.02600
34-1
4.21
25-4
0.858
11- e *-+f*
o . 02603
53-2
4.22
Ca(HCO3)2
u
Calc. by Henry's Law from CO2 concentrations. See also remarks under Ferrous Bicarbonate, p. 336.
These results show that the solution becomes saturated with Ca(HCO3)2 at
about 15 atmospheres pressure of CO2, and it would be theoretically possible to
convert all the CaCO3 to Ca(HCO3)2 by introducing sufficient CO2 at pressures
greater than 15 atmospheres. Under the conditions of the present experiment,
it was calculated that more than 3 months time would have been required for
the complete conversion.
The solubility of calcium carbonate in water saturated with CO2 at one at-
mosphere pressure was found by Cavazzi (1916) to be 1.56 gms. CaCO3 at o°
and 1.1752 gms. at 15°. A supersaturated solution prepared by passing a rapid
stream of CO2 through sat. Ca(OH)2 solution at 15° contained 2.29 gms. CaCO3.
SOLUBILITY OF CALCIUM CARBONATE IN WATER AT 15°. (Tread well and Reuter, 1896.)
(Among the investigators who have reported results upon the solubility of calcium carbonate may
be mentioned, Cossa, 1869; Schloesing, 1872; Caro, 1874; Reid, 1887-88; Irving and Young, 1888; Ander-
son, 1888-89; Engel, 1888; Lubavin, 1892; Pollacci, 1896.)
Gms. per 100 cc. Saturated Solution.
cc. CO2 per 100 cc.
Gaseous Phase
(o° and 760 mm.).
8.94
6.04
Partial Pres
of CO2 in n
Hg.
67.9
45-9
5-45
2.18
41.4
16.6
1.89
14.4
1.72
0.79
i3-i
6
0.41
3-i
0.25
0.08
1.9
0.6
Free CO*.
Ca(HCO3)2.
Ca.
0.1574
0.1872
0.0462
0.0863
0.1755
0.0433
0.0528
0.1597
0.0394
0.0485
O.I54O
0.0380
0.0347
O.I492
0.0368
0.0243
O.I33I
0.0329
O.OI45
0.1249
o . 0308
O.OO47
0.0821
o . 0203
O.OO29
0.0595
0.0147
O.O4O2
o . 0099
0-0385
0.0095
Therefore i liter sat. solution at 15° and o partial pressure of CO2 contains
0.385 gram Ca(HCO3)2. Determinations similar to the above, made in o.i n
NaCl solutions at 15°, are also given. It is pointed out by Johnston (1915), that
although Treadwell and Reuter made very painstaking analyses, their mode of
working did not secure equilibrium conditions, a fact which is borne out by the
lack of constancy of the calculated solubility-product constant.
193 CALCIUM CARBONATE
SOLUBILITY OF CALCIUM CARBONATE (CALCITE) IN WATER IN CONTACT
WITH AIR AT DIFFERENT TEMPERATURES. "
(Wells, 1915.)
(Joplin, Mo., calcite was used. The solutions were kept in a thermostat and
agitated by a current of out-door air filtered through cotton and washed by
water. The CO2 content of the air varied from 3.02 to 3.27 parts per 10,000.
The calcium content of the solutions was determined by titrating with 0.02 n
NaHSO4, using methyl orange as indicator. The solutions were slightly acid
to phenolphthaleine, showing.that the calcium was present chiefly as bicarbonate.)
t°. Cms. CaCOs per Liter.
o 0.081
10 0.070
20 0.065
25 0.056 (0.046)
30 0.052
40 o . 044
50 0.038 (0.029)
Results in parentheses by Kendall (1912). In connection with these it is
stated by Johnston (1915), that assurance is wanting that the partial pressure of
CO2 was the same at both temperatures and the results are, therefore, not neces-
sarily comparable.
SOLUBILITY OF CALCIUM CARBONATE IN WATER AT DIFFERENT TEMPERATURES
AND IN CONTACT WITH AIR CONTAINING DIFFERENT PARTIAL PRESSURES OF
C02.
(Leather and Sen, 1909.)
Results at 15".
Partial
Pressure Gms- per Liter Sol.
Results at 25°.
Pressure Gms. per Liter Sol.
Results at 40°.
Partial
Pressure Gms. per Liter Sol.
CO2 in Gas ' CaCOs.
C02.
C02inGas CaCOs.
C02. '
COz in Gas" CaCOs.
C02. '
Phase.
Phase.
Phase.
0.8
0
• 193
0.117
0.7
0
•159
0
.091
0.6
0.136
0.078
i .5
0
• 193
0.152
1.6
0
.177
o
.III
i .7
0.143
0.085
1.7
o
.238
0.135
4-6
o
•341
o
.208
2.9
0.175
0.106
6.8
0
•445
0.327
7.8
0
.446
0
.301
3-5
0.232
0.169
9.9
0
.627
0.456
16.5
o
•539
o
.522
7
0.284
0.234
13-6
o
.723
0.560
30.1
o
•743
o
•715
14.9
0.384
0.293
14.6
0
.686
0.623
35-5
0
•755
o
.803
22.2
0.427
o 333
31.6
I
.050
1.117
31-7
0.480
0.476
Similar results also given for 20°, 30° and 35°.
The mixtures were constantly agitated at constant temperature. The solid
phase in each case was found to be CaCO3 and it is concluded that Ca(HCO3)2
cannot exist in this solid state above 15°.
In discussing the experiments of Leather and Sen, Johnston (1915) points
out that their method of analysis gives low results for CO2. A calculation of
the data yields very irregular results and the most that can be deduced from
them is that the solubility-product constant of calcite probably decreases some-
what with temperature, becoming apparently about 0.5 X io~8 at 40°.
Data for the solubility of CaCOs in boiling water are given by Cavazzi (1917).
Data for the solubility of calcium carbonate in water containing excess of
carbon dioxide are also given by Seyler and Lloyd (1909). The experiments
were made -at room temperature. Additional experiments showed that small
amounts of CaCl2, CaSO4 or NaHCO3 did not affect the solubility-product con-
stant. Small amounts of Nad, Na2SO4 and MgSO4, containing no ion in common
with CaCOs, resulted in an increase of the total calcium in the solution.
Data for the solubility of calcium carbonate in water, determined by the con-
ductivity method, are given by Holleman and by Kohlrausch and Rose (1893).
CALCIUM CARBONATE
194
SOLUBILITY OF CALCIUM CARBONATE IN AQUEOUS SOLUTIONS OF AMMONIUM
CHLORIDE.
Results at I20-i8°.
(Cantoniand Goguelia, 1905.)
(Flasks>llowed to stand
98 days.)
Cms. per Liter Sat. Sol.
NH4C1.
53-5
100
2OO
CaCOs.
0.423
0.609
0.645
Results at 25°.
(Rindell, 1910.)
(Constant agitation
^ 24 hrs.),.-.
Cms. per Liter Sat. Sol.
Results at 60° for Calcite and Aragonite.
(Warynski and Kouropatwinska,
1916.)
G*ms. per Liter. Cms. per Liter.
NH4C1.
6.7
13-4
26.8
53-5
CaCOs.
0.285
0-373
0.502
0.678
1 NH4C1.
O
1.07
5-35
10.70
26.76
53-52
160.56
Calcite.
0.028
0.164
0-333
0-453
0.664
0-934
I. 21
NH4C1.
O
1.07
5-35
10.70
26.76
53-52
160.56
Aragonite.
0.041
0.184
0.371
0-505
0.728
I.OI5
1.36
SOLUBILITY OF CALCIUM CARBONATE IN AQUEOUS SOLUTIONS OF AMMONIUM
NITRATE AND OF TRIAMMONIUM CITRATE.
laAq. NH4NO3 at 18°. InAq.NH4NO3at25°. In Aq. Triammonium Citrate at 25°.
(Berju andiKosminiko, 1904.)
Gms. per Liter Sat. Sol.
(Rindell, 1910.)
Gms. per Liter Sat. Sol.
(Rindell, 1910.)
Mols. Citrate Gms. CaCOs
per Liter.
0.0625
0.125
0.250
0.500
per Liter.
1.492
2.264
3.980
6.687
NH*NOs. CaCOs. NH4NOs. CaCOs.
o 0.131 5 0.200
5 0.211 10 0.278
10 0.258 20 0.383
20 0.340 40 0.526
4O 0.462
80 0.584
SOLUBILITY OF CALCIUM CARBONATE IN AQUEOUS SOLUTIONS OF MAGNESIUM
CHLORIDE, MAGNESIUM SULFATE, SODIUM CHLORIDE AND SODIUM SULFATE
UNDER CO2 PRESSURE OF Two ATMOSPHERES. (Ehlert and Hempei, 1912.)
Gms. Hv- ^. ^ r,^
Aq. Salt
Solution.
MgCl2.6H2O
«••
Gms. Hy-
drated Salt
per 1000 Gms.
HaO.
Gms. CaCOs . Salt
"SSL* &S ''•
Gms. Hy-
drated Salt
per looo
Gms. H20
Gms. CaCOs
per looo cc.
Solvent.
5
O
2-337
NaCl
5
8
3-740
5
6.1
2.352
"
5
86
3- 783
5
50
3-404
u
5
106.9
3.690
5
86.9
4.083
tc
5
175-6
3-350
5
350
3-301
"
263.4
2.8x1
5
700
2.736
cc
8
35i-2
2.163
5
1150
2.205
MgSO4.7H2O
14
105-3
2.177
5
1725
i .706
u
14
(sat.)
0.914
5
2300 sat.
i .406
Na2S04.ioH20
14
137-7
1 .406
5
28
3.280
"
14
(sat.)
1 .920
NaCl
SOLUBILITY OF CALCIUM CARBONATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AND OF POTASSIUM SULFATE AT 25°. (Cameron and Robinson, 1907.)
Results for Aqueous KCI: " Results for Aqueous K2SO4:
iii coiiuici wnn air.
Gms. per 100 Gms.
Sat. Sol.
atmosphere of CO2.
Gms. per 100 Gms.
Sat. Sol.
:' atmosphere of C02.
Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol. Sat. Sol.
KCI.
0
3-9
7-23
13-82
18.21
26
CaCOa.
0.0013
0.0078
0.0078
0.0072
0.0070
0.0060
KCI.
O
3-9
7-23
13.82
18.21
26
CaCOs.
0.062
0.145
0.150
0.165
0.154
0.126
K2S04.
1. 60
3.15
4-73
6.06
8.88
10.48
CaCOs.
0.0104
0.0116
0.0132
0.0148
0.0192
0.0188
K2S04
0.69
i-37
1.67
2.18
2.99
CaO. '
0.69
0.69
0.47*
0.30*
0.24*
* J5olid phase syngenite.
One liter aqueous solution containing 223.8 gms. KCI dissolves 0.075 gm.
calcite at 60°.
One liter aqueous solution containing 223.8 KCI dissolves 0.093 gm- aragonite
at 60°. (Warynski and Kouropatwinska, 1916.)
195 CALCIUM CARBONATE
SOLUBILITY "OF CALCIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 25°.
Solutions in contact with.
CO2 Free Air. Ordinary Air. CO2atOne Atmos. Pressure.
(Cameron, Bell and Robinson, 1907.) (Cameron and Seidell, 1902.) (Cameron, Bell and Robinson, 1907.)
Cms. per 100 Gms. HzO. Gms. per 100 cc. Sat. Sol. Gms. per 100 Cms. H2O.
NaCl.
CaCOa.
' NaCl.
CaCOs.
NaCl.
CaCOa.
1. 60
o . 0079
I
O.OII2
1.49
0.150
5.18
0.0086
4
O.OI4O
5-69
0.160
9-25
o . 0094
8
0.0137
II. 06
0.174
11.48
O.OIO4
10
0.0134
15.83
0.172
16.66
0.0106
15
O.OII9
19.62
0-159
22.04
O.OII5
20
0.0106
29.89
0.123
30-50
O.OII9
25
0.0085
35-85
0.103
Data for the solubility of calcium carbonate in aqueous solutions of mixtures
of sodium chloride and sodium sulfate in contact with air and with CO2 are
given by Cameron, Bell and Robinson (1907).
Data for solubility of CaCO3 in aqueous NaCl and other salt solutions, de-
termined by boiling and cooling the solution, are given by Gothe (1915).
Data for the solubility of mixtures of calcium carbonate and calcium sulfate in
aqueous solutions of sodium chloride at 25°tare given by Cameron and Seidell (1901 ).
Data for the solubility of mixtures of calcium carbonate and calcium sulfate
in aqueous solutions of mixtures of sodium chloride and sodium sulfate at 25°,
in contact with air and with CO2, are given by Cameron, Bell and Robinson (1907).
One liter aqueous solution containing 175.5 gms. NaCl dissolves 0.062 gm.
calcite at 60°.
One liter aqueous solution containing 175.5 gms- NaCl dissolves 0.071 gm.
aragonite at 60°, (Warynski and Kouropatwinska, 1916.)
SOLUBILITY OF CALCIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM
HYDROXIDE IN CONTACT WITH CO2 FREE AIR.
(LeBlanc and Novotny, 1906.)
Gms. CaCOs per Liter Sat. Sol.
Water 0.0128 0.0207
About o . oooi n NaOH 0.0087 0.0096
" o.ooiow " 0.0042 0.0069
" o.oioow " 0.0042 0.0057
Data on the equilibrium in aqueous solutions of CaCO3, Na2CO3 and NaOH
are given by Wegscheider and Walter (1907).
SOLUBILITY OF CALCIUM CARBONATE iNAQUEOUs.SoLUTiONs OF SODIUM SULFATE.
Solutions in contact with:
CO2 Free Air at 25°. Ordinary Air at 24°.
(Cameron, Bell and Robinson, 1907.) (Cameron and Seidell, 1902.)
Gms. per IPO Gms. HsO. Gms. Na.SCu S^E'SL?
Na2SO<. CaCOs. ^ per Liter. ECa(HCO8),.'
0.97 0.0151 5 0.175
1.65 0.0180 10 0.232
4.90 O.O262 2O 0.277
12.69 0.0313 40 0.332
14.55 0.0322 80 0.400
19.38 0.0346 I5O 0.510
23.90 0.0360 250 0-725
Freezing-point data for mixtures of calcium carbonate and calcium chloride
are given by Sackur (1911-12).
CALCIUM CHLORATE
196
CALCIUM CHLORATE Ca(ClO3)2.2H2O.
loo grams saturated aqueous solution contain 64 grams Ca(ClO3)2 at 18°.
Density of solution is 1.729. (Mylius and Funk, 1897.)
CALCIUM CHLORIDE CaCl2.
SOLUBILITY IN WATER
(Roozeboom — Z. physik. Chem. 4, 42, '89; see also Mulder; Ditte — Compt. rend. 92, 242, '81; Engel
— Ann. chim. physic. [6Ji3, 381, '88; Etard — Ibid, [7] 2, 532, '94.)
Cms. CaClj per
100 Gms.
Solid
Phase.
-55
-2$
O
10
20
Water. Solution.
42.5 29.8 Ice + CaCl2^H2O
50.0 33.3 CaCl2.6H20
59-5 37-3 CaC1*-6H*°
65.0 39.4 CaCl2.6H2O
42.7 CaCl2.6H20
50.7 CaCl2.6H2O
47.6 CaCl2.4H2Oa
50.1 •4H2Oa+.6H20
53.4 -4H2Oa.
5I.I CaCl2.4H200
0 wiH2O /3 + .6H2O
74-5
3O.2 IO2-7
20 91.0
29.8 100.6
40 II5-3
20 104.5
29.2 112. 8
35 I22-5
38.4 127.5
45-3 130-2
Density of saturated solution at o° = 1.367, at 15° = 1.399, 'at 18° = 1.417;
at 25° = 1.47.
SOLUBILITY OF CALCIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID AT o°.
(Engel, 1887.) _
53
55.0
56.0 wtH2Q/3+CaCl2.2H20
56.6 ^H2O a + CaCl2.2H2O
Gms. CaCl2 per
t°.
100
Gms.
Solid
Water.
Solution.
ase.
60
136.8
57-8
CaCl2.2H2O
70
I4I.7
58.6
CaCl2.2H2O
80
147.0
59-5
CaCl2.2H2O
90
152 .7
60.6
CaCl2.2H2O
100
159.0
61 .4
CaCl2.2H2O
120
173.0
63-4
CaCl2.2H2O
I4O
I9I.O
65.6
CaCl2.2H2O
160
222-5
69.0
CaCl2.2H2O
170
255-0
71.8
CaCk-aHaO
175-5
297.0
74-8;
( CaClz.2H20
t -t CaCla-iizC
180
300.0
75-o
CaCl2.H3O
200
3II.O
75-7
CaCl2.H20
235
332-0
76.8
CaCl2.H2O
260
347-0
77.6
CaCl2.H20
CaCb.
HC1.
U0 01 JH.L. OU1.
' CaCh.
HC1.
51-45
0
1.367
29.84
I5-84
1.283
46.45
3-32
1-344
20. 1 2
23-I5
I.25O
42.80
5-83
1.326
11.29
34.62
1.238
36.77
10.66
1.310
SOLUBILITY OF MIXTURES OF CALCIUM CHLORIDE, MAGNESIUM CHLORIDE AND
CALCIUM MAGNESIUM DOUBLE CHLORIDE (TACHHYDRITE).
(Van't Hoff and Kenrick, 1912.)
Gms. per 100 Gms.
CaCl2.
MgCk
41.2
31-6
57-i
26
54-5
28.4
o
85.63
32-3
17.9
80. i
16.1
88.7
7.24
16.7
21-95
28.2
116.7
25
28.2
28.2
Tachhydrate = 2MgCl2.CaCl2.i2H2O.
100 grams H2O dissolve 63.5 grams CaCl2 + 4.9 grams KC1 at 7° (M).
100 grams H2O dissolve 57.6 grams CaCl2 + 2.4 grams NaCl at 4° (M).
loo grams H2O dissolve 59.5 grams CaCl2 + 4.6 grams NaCl at 7° (M).
100 grams H2O dissolve 72.6 grams CaCl2 + 16 grams NaCl at 15° (R).
(M) = Mulder. (R) = Rudorff.
Solid Phase.
MgCU.6H20-r-CaCl2.6H20
" " +Tachhydrite
Tachhydrite+MgCl2.6H2O
+ " +MgCl2.4HsO
+CaCl2.6H2O +CaCl2.4H2O
+CaCl2.4H20
CaCl2.6H204-CaCl2.4H20
197 CALCIUM CHLORIDE
SOLUBILITY OF CALCIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 25° AND VICE VERSA.
(Cameron, Bell and Robinson, 1907.)
1M
Sat.fol.
I.444I
I-365I
1.3463
1.2831
Gms. per 100 Cms. HzO
'• Solid
Phase.
CaCl2.6H2O
" +NaCl
NaCl
dtt (
Sat. Sol.
1-2653
1.2367
I . 2080
I . 2030
Gms. per 100 Gms. HzO
• Solid
* CaCl2.
84
78.49
58.48
53-47
36.80
NaCl.
o
1.846
1.637
1.799
7-77
CaCl2.
30.08
19-53
3-92
O
NaCl.
10.70
18.85
32.48
35-80
' Phase.
NaCl
SOLUBILITY OF CALCIUM CHLORIDE IN AQUEOUS ALCOHOL AT ROOM TEMPERATURE.
(Bodtker, 1897.)
Vol. Gms. Vol. Gms.
Solution Used. Per Cent CaCk per Solution Used. Per Cent CaClsper
Alcohol. 5 cc. Sol. Alcohol. 5 cc. Sol.
15 Gms. CaCl2.6H2O 15 Gms. CaCl2.6H2O+2o cc.:
+ 20 cc. alcohol 92.3 1.430 alcohol + 2 Gms. CaCl2 99.3 1.561
15 Gms. CaCl2.6H2O + 3 99-3 i • 59°
+ 20 cc. alcohol 97.3 1.409 " +4 " 99.3 1.641
15 Gms. CaCl2.6H2O " +5 " 99-3 1.709
+ 20 cc. alcohol 99.3 1.429
15 Gms. CaCl2.6H2O
+ 20 cc. alcohol
+ i Gm. CaCl2 99.3 1.529
SOLUBILITY OF CALCIUM CHLORIDE IN AQUEOUS SOLUTIONS OF ACETONE
AT 20°.
(Frankforter and Cohen, 1914.)
Measured amounts of acetone were added to known solutions of CaCl2 in water,
until opalescence, indicative of the separation of a second liquid layer, was ob-
served. The composition of a large number of such mixtures gives the limiting
values for the binodal curve of the system. Tie lines were also determined in
several instances by using such quantities of the three components that an ade-
quate amount of each layer would be formed to permit the determination of the
CaCl2 in it. The points thus located on the curve fix the tie lines, and from them
the approximate position of the plait point can be estimated.
Points on the Binodal Curve Composition of Points Representing
at 20°. Tie Lines at 20°.
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer.
Acetone.
Cadi.
Acetone.
CaCl2. Acetone. CaCl2.
9
40.5* /(solid phase
90.2
0.186 28.5 16.61
22.7
38.l6tf CaCl2)
83-3
0.628 34.6 12.97
20.8
31.2
8l
o . 948 40 10 . 6
2O. 2
28
78.5
1.321 43-5 9-36
21
24.4
60
5 (plait point) 60 5
23
21.1
Points on
the Binodal Curve at Different
25
19.2
is 6
Temperatures.
35
•*• 0 • w
12.8
Gms. per loo^Gms. Sat. Sol.
40
'
Acetone. CaCl2.
45
8.8
5
3I.09 I5-52
50
7-4
10
22.77 23.64
55
6.1
15
31.09 I5-52
60
5
18
30-58 15-27
65
70
3-9
2.8
25
25
21.44 22.25
29.83 14.89
75
1.8
30
20.99 21.79
80
i
30
29.27 14.62
85
35
21.14 20.91
9°
O.2
35
28.59 14-29
95
O.I
40
19.83 20.58
Point on solubility curve, t Quadruple point. 4°
27.90 13.93
CALCIUM CHLORIDE 198
SOLUBILITY OF CALCIUM CHLORIDE IN A SATURATED SOLUTION OF SUGAR AT
31-25°.
. (Kohler, 1897.)
100 grams saturated solution contain 42.84 grams sugar + 25.25 grams CaCl2,
or 100 grams water dissolve 135.1 grams sugar + 79.9 grams CaCl2.
100 gms. 95% formic acid dissolve 43.1 gms. CaCl2 at 19°. (Aschan, 1913.)
loo cc. anhydrous hydrazine dissolve 16 gms. CaCl2 at room temp.
(Welsh and Broderson, 1915.)
ioo gms. propyl alcohol dissolve 10.75 S1118- CaCl2 (temp.?). (Schlamp, 1894.)
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES OF CALCIUM CHLORIDE AND OTHER SALTS.
CaCl2+CaF2 (i) (2)
CaCl2+CaI2 (i)
CaCl2+CaO(3)
CaCl2+CaSi03 (4)
CaCl2+CuCl (5
(3)
5)
(i) = Ruff and Plato, 1903; (2) = Pla
= Menge, 1911; (6)= Sandonnini, 1911;
reng, 1914; (10) = Schaefer, 1914.
CaCl2+PbCl2 (5) (6) (7)
CaCl2+LiCl (7) (8)
CaCl2+MgCl2 (5) (6)
CaCl2+MnCl2 (6) (7)
CaCl2+KCl (5) (3)
CaCl2+NaCl (5) (3)
CaCl2+AgCl (5)
CaCl2+SrCl2 (6) (7) (3) (10)
CaCl2+SrO (3)
CaCl2-fTlCl (9) *
CaCl2+SnCl2 (5)
CaCl2+ZnCl2 (5)
Plato, 1907; (3) = Sacfcur, 1911-12; (4) = Karandeeff, 1910; (5)
(7) = Sandonnini, 1913; (8) = Sandonnini, 1913; (9)= Kor-
CALCIUM CHLORIDE ACETAMIDATE CaCl2.3CH3CONH2.
SOLUBILITY IN ACETAMIDE AT VARIOUS TEMPERATURES, DETERMINED BY THE
SYNTHETIC METHOD.
(Menschutkin, 1908.)
t° /-
Gms. per
Sat.
too Gms.
So1- Solid
Gms. per ioo Gms.
^0 Sat. Sol.
Solid
CaCl2.3CH3-l_rarl ' Phase.
CONH2 /-CaCl2-
CaCl2-3CH3-\ r r,
CONH2 j=CaC!2.
Phase.
82 m. pt.
0
0 CHaCONIfc
IOO
65.6
25-3
1-3
78
8
3.1 "
150
70-5
27.1
"
74
15-4
5-9 "
165
74.8
28.8
"
66
27
10.4 "
175
80.6
31
"
54
39-2
I5.I '«
180
85-5
32.9
it
46 Eutec.
45
17.3 " +1.6
184
90-5
34-8
"
58
48-5
18.7 1.6
186 tr.
pt. 94.5
3^-4
" +CaCl2(?)
62
54-5
21
200
97-5
37-5
CaCla(?)
64 tr. pt.
62.1
23.9 1.6+1.3
2IO
IOO
38.5
«
1.6 = CaCl2.6CH3CONH2. 1.3 = CaCl2.3CH3CONH2
CALCIUM CHLORIDE ACETIC ACIDATE CaCl2.4CH3COOH.
SOLUBILITY IN ACETIC ACID AT VARIOUS TEMPERATURES, DETERMINED BY THE
SYNTHETIC METHOD.
(Menschutkin, 1906.)
Gms. per ioo Gms.
Sat. Sol. SoUd
Phase.
CaCl2.4CH3-l ran
COOH /-CaCl2.
16.2
m. pt. o o
15
18 5-7
14
27 8.5
13
34 10.7
II. I
Eutec. 42 13-3
30
47.6 15
35
5o 15-8
1.4
t°.
CHsCOOH
40
45
60
" +1-4 65
1.4 70
73 m. pt.
CaCl2.4CH3COOH.
Gms. per ioo Gms.
Sat. Sol.
Solid
Phase.
CaCWCHs-l
COOH /
= CaCl2.
54-7
17-3
1*4
63
19.9
"
69.5
21-9
"
79-5
25.1
"
84-5
26.7
"
91 .2
28.8
H
IOO
31-6
•
199
CALCIUM CHLORIDE
CALCIUM CHLORIDE ALCOHOLATES CaCl2.3CH3OH, CaCl2.3C2H5OH.
(The compounds were prepared by mixing anhydrous CaCl2 with the alcohbf.
In the case of the methyl alcohol compound, the tri CH3OH salt crystallizes
above 55°, the tetra salt below this temperature.)
SOLUBILITY OF EACH IN THE RESPECTIVE ALCOHOL AT VARIOUS TEMPERATURES,
DETERMINED BY THE SYNTHETIC METHOD.
(Menschutkin, 1906.)
Results for CaCl2.3CH3OH. Results for CaCl2.3C2H5OH.
Gms. per 100 Gms. Gms. per 100 Gms.
• o Sat. Sol. Solid *<, Sat. Sol. Solid
Gms. per 100 Gms.
to Sat. Sol.
CaCl2.3CH3OH - CaCl2.' CaCU-sCHaO]
H = CaClz. CaCl2.3C2HsOH = CaCl2
0
33
O
17-85 1-4 95
66
3
35-
5 1.3
O
34-8
iS-5
10
37
6
20.15
"5
70
3
37-
6
2O
46
20.5
2O
42
2
22.6
135
75
2
40.
3
40
58.7
26.1
30
47
25.2
155
81
8
43-
8
60
73
32.5
40
S2
27.8
165
86
2
46.
2 "
70
80.8
36
5°
57
3
30-7
' 170
89
5
47-
9
80
86.8
38.7
55
60
32.1 174
93
5
50.
i "
85
89.2
39-7
56
61
3
32.8 « 177*
IOO
53-
6
90
91.9
40.8
55
60
5
32.4 "+1.3 190
55-
7 i.i(?)
95
96.2
42.8
75
63
i
33-8 1.3 215
57-
7 "
97*
IOO
44-5
14 = CaCl2.4CH3OH. 1.3
* M. pt.
CaCl2.3CH3OH, i.i = CaCl2.CH3OH.
CALCIUM CHROMATE CaCrO4.
SOLUBILITY OP THE SEVERAL HYDRATES IN WATER.
(Mylius and Wrochem — Wiss. Abh. p. t. Reichanstalt 3, 462, 'oo.)
-. o Gms. CaCrO4 per 100 Gms. Mols. CaCrO4
* • i — ; • — — — ; > per 100 Mols.
Water. Solution. H2O.
SoHd Phase, o CaCrO4.2H2O. (Monoclinic.)
0
17-3
14-75
2.O
18
16.68
14-3
i-93
20
16.6
14.22
i-93
30
16-5
I3-89
1-85
45
14-3
I2-53
1-65
Solid Phase, ft CaCr04.2H20 (Rhombic.)
o 10.9 9.8 i
18 11.5 10.3 i
40 1 1 . 6 10 . 4 i
Solid Phase, CaCrO4.H2O.
•25
•33
•34
0
13.0
"•5
1.50
18
10.6
9.6
I .22
25
10.0
9.1
*•*$
40
8-5
. 7-8
0.98
60
6.1
5-7
0.70
75
4-8
4.6'
0.56
IOO
3-2
3-i
o-37
f.c
Jms. CaCrO4 per TOO Gms. ^
[ols.CaCr04
er TOO Mols.
H20.
Water.
Solution.' *
Solid Phase,
CaCr04.iH20
o
7-3
6.8
0.84
18
4-8
4.4
0.51
3i
3-84
3-7
0.44
38
•5 2.67
2,6
0.31
5o
1.63
1.6
0.19
60
1-13
i.i
0.13
ICO
0.81
0.8
O.O9
Solid Phase, CaCrO4.
O
4-5
4-3
0.52
18
2.32
2.27
0.27
31
2 .92
1.89
O-22
5o
1. 12
i. ii
0.13
60
0.83
0.82
O.II
70
0.80
0.79
O.OQ
IOO
0.42
0.42
0.05
Densities of the saturated solutions of the above several hydrates
at 18° are: a CaCrO4.2H2O, 1.149; £ CaCrO4.2H2O, 1.105; CaCrO4.H2O,
1.096; CaCrO4.iH2O, 1.044; CaCrO4, 1.023.
loo cc. 29% alcohol dissolve 1.206 grams CaCrO4.
loo cc. 53% alcohol dissolve 0.88 gram CaCrO4.
(Fresenius — Z. anal. Chem. 30, 672, '91.)
CALCIUM CINNAMATES 200
CALCIUM CINNAMATE Ca(C6H6.CH:CHCOO)2.3H2O.
SOLUBILITY OF CALCIUM CINNAMATE AND ITS ISOMERS IN SEVERAL
SOLVENTS.
Name of Salt.
Calcium Cinnamate
Formula.
Ca(C6H6CH:CHCOO)1.3HiO
Ca(C9H702)2.3H20
Isocinnamate
M
Allocinnamate
«
tt
Hydrocinnamate
(i) = De Jong, 1909; (2) = Tarugi and CheccnC 1901;
1903; (s)
. and Garner, 1903.
(3)
Gms. Anhy-
Solvent.
t°.
drous Salt per
100 Gms.
Solvent.
Water
2
0.19(1)
"
15
0.2l(2)
"
26
100
0.24(1)
1.15(2)1
"
20
23-8 (3)
Acetone
2O
19-6 (3)
M
2O
2 (3
Water
2O
10.2 (4
Acetone
18
2-7 (5
u
14
0.19(5)
"
19
0.21(5)
Water
27
4.25(3)
Acetone
25
3-3 (3)
= Michael,
1901; (4
)_= Liebermann,
CALCIUM CITRATE Ca3(C6H6O7)2.4H2O.
SOLUBILITY IN WATER AND IN ALCOHOL AT 18° AND AT 25°.
(Partheil and Hubner, 1903.)
Solvent.
100 Gms. Solvent at:
Water
Alcohol (Sp. Gr. 0.8092 = 95%)
18°.
0.08496
0.0065
25 •
0.0959
0.0089
EQUILIBRIUM IN THE SYSTEM CALCIUM OXIDE-CITRIC ACID-WATER AT 30°.
(van Itallie, 1908.)
The compositions of the solid phases were determined by the " Rest Method '
of Schreinemakers (1903). The results are presented in the triangular diagram
and it was necessary to select the fictitious compound CeHsOj.i^HsO instead of
CeHgO? in order to keep the citrate component within the limits of the diagram.
This is in harmony with the choice of anhydrides as components in the inorganic
oxy acid systems.
Gms. per 100 Gms.
' Sat. Sol.
QHsCh.
CaO.
5*5.86
0
54-8
OK 24
55-4
0-35
53-7
0.40
48.3
0.52
42.6
O.6O
38.5
0.77
36.5
0.70
34-8.
0.77
27-5
0-45
Solid Phase.
+C«H«O7Ca.4H2O
Gms. per 100 Gms. Sat.
Sol.
^StjO
CaO.
20.3
0.35
I6.3
0-33
12-5
0-39
8-3
0.28
5-2
0.25
4.1
O.2O
3-2
0.20
2.4-0
0.2I-O.I3
0.18
0.24
0
O.II3
Solid Phase.
Quadruple pt.
Quadruple pt.
Ca(OH),
CALCIUM Potassium FERROCYANIDE CaK2Fe(CN)6.3H2O.
100 parts H2O dissolve 0.125 part salt at 15°, and 0.69 part at boiling-point.
(Kunheim and Zimmerman, 1884.)
ioo gms. H2O dissolve 0.41 gm. CaK2Fe(CN)6 at 15-17°.
(Brown, 1907.)
201 CALCIUM FLUORIDE
CALCIUM FLUORIDE CaF2.
One liter sat. aqueous solution contains 0.016 gm. CaF2 at 18° and 0.017
gm. at 26°.
One liter sat. aqueous solution contains 0.0131 gm. fluorspar at o°, 0.0149
gm. at 15°, 0.0159 gm. at 25° and 0.0167 gm. at 40°. (Kohlrauscb, 1904-05, 1908.)
Freezing-point data for mixtures of calcium fluoride and calcium iodide are
given by Ruff and Plato (1903) and for mixtures of calcium fluoride and calcium
silicate by Karandeeff (1910).
CALCIUM FORMATE Ca(HCOO)2.
SOLUBILITY IN WATER.
(Lumsden, 1902; see also Krasnicki, 1887.)
Cms. Ca(HCOO)2 per 100 Gms. Cms. Ca(HCOO)» per 100 Gms.
Water. Solution. Water. Solution. "
o 16.15 I3-9° 60 17-50 14.89
20 16.60 14.22 80 17-95 15-22
40 17.05 14.56 100 18.40 15.53
Results in good agreement with the above are given by Stanley (1904).
CALCIUM GLYCEROPHOSPHATES a = OH.CH2.CH(OH)CH2.OPO3Caf
0 = OH.CH2.CH.OPO3Ca.CH2OH.
SOLUBILITY OF CALCIUM a. GLYCEROPHOSPHATE IN WATER.
(Power and Tutin, 1905; Couch, 1917.)
to Gms. CaCaHrOeP ^o Gms. CaCsHrOeP
per loo Gms. Sat. Sol.! per 100 Gms. Sat. Sol.
05 40 3-5
10 4.6 60 2.7
20 5.2 80 1.8
25 5 100 0.9
Results varying from 1.7 to 5.4 gms. per 100 gms. sat. solution at or near
1 8° are given by Rogier and Fiore (1913), Willstaetter (1904) and King and
Pyman (1914). It is pointed out by Couch, however, that since the solubilities
of the a and ft isomer differ, and also that the commercial product contains
both isomers, variable results will be obtained, depending on the composition of
the product and the method used for determining the solubility. These authors
also show that increasing amounts of alcohol in the solvent decrease the solu-
bility of calcium glycerophosphate.
i oo grams H2O dissolve i .66 grams calcium /3 glycerophosphate at 20°. (Couch, 1917.)
The results of King and Pyman (1914) are: 1.4 gms. at 13° and I gm. at 15°.
CALCIUM HEPTOATE (Oenanthate) Ca[CH3(CH2)5COO]2.HaO.
SOLUBILITY IN WATER.
(Lumsden, 1902; see also Landau, 1893; Altschul, 1896.)
t . o°. 20°. 40°. 60°. 80°. '100*
Gm. Ca(C7Hi3O2)2 per
100 gms. solution 0.94 0.85 0.81 0.81 0.97 1.24
CALCIUM HYDROXIDE Ca(OH)«.
Recent determinations of the solubility of calcium hydroxide in water, agree-
ing fairly well with the average results given in the table on next page, are given
by Bassett, Jr. (1908), Moody and Leyson (1908), Chugaev and Khlopin (1914)
and Seliwanow (1914).
One liter sat. aqueous solution contains 0.305 gm. CaO at 120°, 0.169 Sm- at
150° and 0.084 gm. at 190°. (Herold, 1905.)
One liter of aqueous 5.2% NH3 solution dissolves 0.81 gm. Ca(OH)2 at about
20°. (Konowalow, *899&.,>
CALCIUM HYDROXIDE 202
CALCIUM HYDROXIDE Ca(OH)2.
SOLUBILITY IN WATER.
(Average curve from the results of Lamy, 1878; Maben, 1883-84; Herzfeld, 1897, and Guthrie ,^19.01.)
Grams per 100 Grams EhO. - , 0 "Grams per too Grams H2O.
*' ' Ca(OH)2. CaO. ' Ca(OH2). CaO.
o 0.185 0.140 50 0.128 0.097
10 0.176 0.133 60 0.116 0.088
20 0.165 °-I25 7° 0.106 0.080
25 °-I59 0.120 80 0.094 0.071
30 o^SS 0.116 90 0.085 0.064
40 0.141 0.107 I0° 0.077 0.058
SOLUBILITY QF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OP
AMMONIUM CHLORIDE AT 25°.
(Noyes and Chapin — Z. physik. Chem. 28, 520, '09.)
Millimols per Liter. Grams per Liter of Saturated Solution.
NH^Cl. Ca(OH)2. NI^Cl. ClT(OH)2 = CaO.
o.oo 20.22 o.oo 1-50 1.13
21.76 29.08 1-165 2.l6 1.63
43.52 39-23 2.330 2.91 2.20
83-07 59 -68 4-447 4-42 3-45
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF
CALCIUM CHLORIDE.
(Zahorsky — Z. anorg. Chem. 3, 41, '93; Lunge — J. Soc. Chem. Ind. u, 882, '92.)
Concentration Grams CaO Dissolved per 100 cc. Solvent at:
— —~ ~
itions,Wt.%. f
20°.
40°.
60°.
80°.
100°. '
0
o.
1374
0
.Il62
0
.1026
0
.0845
0
.0664
5
o.
1370
0
.Il6o
0
.1020
0
.0936
0
.0906
10
o.
1661
0
.1419
0
•1313
o
.1328
0
.1389
IS
o.
*993
o
.I78l
0
.1706
o
.1736
0
.1842
20
o.
1857*
0
.2249
0
.22O4
0
.2295
o
•2325
25
o.
1661*
o
.3020*
0
.2989
0
.3261
o
.3710
30
o.
1630*
o
.3680*
o
.3664
0
.4122
0.4922
* Indicates cases in which a precipitate of calcium oxychloride separated and thus removed some of
the CaCh from solution.
The results in o% CaCh solutions, i.e., in pure water, are high wken compared with the average
results given above.
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF CALCIUM
CHLORIDE AT 25°.
(Schreinemakers and Figee, 1911.)
JC&Clt.
5.02
CaO.
O . IOI Ca(OH)2
CaCl2.
33-21
CaO.
0.245
> ooiiu imase.
CaCl2.4CaO.i4H2O
10
O.II5
"
33-72
0.254
" +CaCl2.Ca0.2H2O
15.14
0.140
"
34.36
0.173
CaCl2.CaO.2H2O
18.15
0.148
" +CaCl2.4CaO.i4H2O
38.61
O.O6O
"
18.01
0.152
CaCl2.4CaO.i4H2O
41 .32
0.048
M
21.02
0.147
"
44.30
O.O3O
"
28.37
0.170
«
44.61
0.029
" +CaCl2.6H20
32.67
O.225
Ca(OH)2?
44-77
CaCl2.6H20
Data for the above system at 10°, 25°, 40°, 45°, 48°, and 50° are given by
Milikau (1916).
Data for the solubility of calcium hydroxide in aqueous calcium iodide solu-
tions at 25° are also given by Milikau.
203
CALCIUM HYDROXIDE
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF CALCIUM
NITRATE AT 25° AND AT 100°.
(Bassett and Taylor, 1914; see also Cameron and Robinson,
Results at 25°.
Gms. per 100 Gms.
Sat. Sol.
Results at 100°.
Gms. per 100 Gms.
Solid Phase.
, per i
Sat. S
Sol.
Solid Phase.
Results at 100° (Con.).
Gms. per 100 Gms.
Sat. Sol. solid Phase.
'CaO.
Ca(NO,)2.
CaO.
Ca(NO3)2. CaO.
Ca(N03)2.'
O.II50
o
Ca(OH)2 0.0561
O
Ca(OH)» . 576
58
.67
(
'a2N2Ct7.2H2O
0.0978
4-
836
0.0550
2
.42 " .348
60
•44
"
0.1074
9-
36
" 0.0624
4
.91 " .167
62
.82
H
O.H93
77
" O.IIIO
15
•39 " -077
66
•44
"
0.1444
22.
46
" O.I2OO
16
. 10 " . 141
69
.12
"
0.1650
27.
83
0.155
21
.86 "
I
" + a very
0.1931
32-
94
0.269
33
.03 " 1.252
70
.60
. little Caj-
0.2579
.40.
66
" 0.480
42
.26
I
NiOr.ilbO
o . 3060
44-
44
0.973 50
•94
* I . 203
70
.40
(
o. 2802
45-
28 Ca2NjOr.3H20 1.261
53
•75
1.103
71
•44
"
0.2314
47-
79
1-477
55
.40
0-937
73
•85
M
0.1894
51-
07
.476
55
•43
0.849
75
•74
"
0.1659
53-
20
" 3
.491
55
•65
• 0.815
76
•94
"
o . 1486
55-
25
"
•635
56
•89 I
+Ca2N2O;.- o . 804
77
.62
Ca(NO,),
0.0836
57-
72 Ca(NOs)2.4H2O
.686
57
.03 S aHzO 0.412
77
•74
"
0
57-
98
M
.596
57
.91 Ca2N2O7.2H2O 0
78
•43
"
Cerasine wax bottles were used and more than 6 months constant agitation
allowed for attainment of equilibrium at 25° and 4-14 days at 100°.
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF CALCIUM
SULFATE AT 25°.
(Cameron and Bell, 1906.)
Gms. per 100 cc. Sat. Sol.
CaO.
0.1166
0.1141
0.1150
0.1215
0.1242
0.1222
Solid
Phase.
Ca(OH)2
Gms. per 100 cc. Sat. Sol.
CaSO4.
O
0.0391
0.0666
0-0955
O.I2I4
0.1588
The mixtures were constantly agitated at 25° for two weeks.
CaSO4.
CaO.
0.1634
0.0939
0.1722
0.0611
0.1853
0.0349
O.IQiS
0.0176
o . 2030
0.0062
0.2126
0
Solid
Phase.
CaS04.2H«0
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AND OF SODIUM CHLORIDE.
(Cabot, 1897.)
- In KC1 Solutions.
Gms. of the
Chloride
Gms. CaO per Liter at:
per Liter. .
' o°. 15°.
99°.
O
1.36 I.3I
0.635
30
I.70I 1.658
0.788
60
1.725 1.674
0.876
120
I.7l8 I. 606
0.894
240
I . 248 I . 199
0.6l7
320
... ...
In NaCl Solutions.
Gms. CaO per Liter at:
0°.
15°.
99°.
1.36
1.31
0-635
1.813
1-703
0.969
1.824
I .004
1.86
1.722
I.OI5
i .37
1.274
0.771
1.054
0.929
0.583
Results in harmony with the above for the solubility of calcium hydroxide
in aqueous solutions of potassium chloride at 50°, are given by Kernot, d'Agostino
and Pellegrino (1908).
CALCIUM HYDROXIDE
204
SOLUBILITY OF LIME IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE ALONE AND
CONTAINING SODIUM HYDROXIDE.
(Maigret, 1905.)
Gms. CaO per Liter of Solution.
tier liter Without o-89.NsOH 4 .09 .NaOH
' NaOH. per Liter. per Liter.
0.22
o-SS
0
•3
0.8
5
•4
0.9
10
.6
I.O
25
•7
i.i
5°
.8
1-25
75 ,
•9
1.4
100
.85
1.4
c Naa Gms. CaO per Liter of Solution.
per Liter Without o.8g.NaOH 4-oo.NaOH
' NaOH. per Liter. per Liter.
150 1.65 1.25 0-44
175 1.6 1.2
182 1.6 1.2
225 1.4 i.o
250 1.3 0.9
300 I.I 0-7 0.22
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF
SODIUM HYDROXIDE.
(d'Anselme — Bull. soc. chim. [3] 29, 938, '03.)
Concentration of NaOH:
Normality.
Gms. per Liter
0
O
N/ioo
0-4
N/25
1.6
N/i5
2.66
N/8
S-oo
N/5
8.00
N/2
20-00
Grams CaO per Liter Sat. Solution at:
20°.
50°.
70°.
100°.
I.I70
0-94
0.880
0.65
0-75
o-53
0-54
o-3S
o-57
o-3S
0.225
0.14
o-39
0.18
0.20
O-o6
o.n
0.04
0.05
o.oi
o.n
0-02
O-OI
trace
0.02
trace
o.oo
o.oo
For results upon mixtures of calcium hydroxide and alkali carbonates
and hydroxides, see Bodlander — Z. angew. Chem. 18, 1138, '05.
SOLUBILITY OF, CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF
GLYCEROL AT 25°.
(Herz andKnoch — Z. anorg. Chem. 46, 193, '05; for older determinations, see Berthelot — Ann. chim
phys. [3] 46, 176; and Carles — Arch. Pnarm. [3] 4, 558, '74.)
Density of
Solutions
Wt. per cent
Glycerine
in Solution.
Millimols
*Ca(OH)2per
i oocc. Solution.
Gms. per 100 cc. Solution.
Ca(OH)2
- CaO. "
.0003
o.o
4-3
0.1593
0.1206
.0244
7-15
8-13
0.3013
0.2281
•0537
20-44
14.9
0.5522
0.4180
.0842
31-55
22.5
0.8339
0.6313
•H37
40.95
40.1
1.486
1.125
•J356
48.7
44.0
1.631
1.234
.2072
69.2
95-8
3-550
2.687
Data tor the solubility of calcium hydroxide in aqueous solutions of phenol
at 25° are given by van Meurs (1916).
205
CALCIUM HYDROXIDE
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF GLYCEROL
AND OF CANE SUGAR AT 25°.
(Cameron and Patten, 1911.)
In order to obviate the uncertainties due to the presence of a large excess of
the solid phase in contact with the solutions, the clear liquids, saturated at o°,
were decanted from the solid and slowly brought to 25° and constantly agitated
at this temperature, until equilibrium with the finely divided solid phase, which
separates at the higher temperature, was reached.
Results for Glycerol Solutions. Results for Sugar Solutions.
da of Gms. per TOO Gms. Sat. Sol. Solid d* of Gms. per 100 Gms. Sat. Sol. Solid
Sat. Sol. "~
Ca(OH)2.
CsH5(OH)3. Pnase- bat.bol.
Ca(OH)2. CwHaOu
Phase.
0
-983
0
.117
0
Ca(OH)«
0
.188
0
.62
Ca(OH)j + Sugar
I
.008
O
.178
3
.50
.021
0
•730
4
.82
"
0
•413
15-59
•037
I
•355
7
•50
"
I
.042
O
.48
17
.84
.067
3
.21
ii
.90
«
I
.088
0
.88
34
.32
.109
5
-38
17
.42
"
I
.149
I
•34
55
.04
.123
6
.07
19
.86
"
SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF CANE SUGAR
AT 80°.
(von Ginneken, 1911.)
Gms. per 100 Gms. Sat. Sol.
CaO.
O.II7
0.189
0.230
Sugar.
4.90
9.90
14-75
Solid
Phase.
Ca(OH)5
Gms. per 100 Gms. Sat. Sol.
CaO. Sugar.
0.358 19.50
0.548 24.60
I.OI7 29.70
Solid
Phase.
Ca(OH),
SOLUBILITY OF LIME IN AQUEOUS SOLUTIONS OF SUGAR.
(Weisberg — Bull. soc. chim. [3] 21, 775, '99.)
The original results were plotted on cross-section paper and the
following table constructed from the curves.
ist series, t° = i6'-i7°.
Jms.
per 100 Gms.
Solution.
G. CaO per 100
Gms. Sugar in Sol.
Sugar. CaO.
I
0.30
35-o
2
0.56
28.7
3
0.85
28.0
4
1. 12
27.7
5
1.40
27-5
6
1.65
27-5
8
2 .22
27-5
10
2.77
27-5
12
3-27
27-5
14
3-85
27-5
2d, series t° =
15°.
rms. per 100 Gms.
Solution.
G. CaO per 100
Gms. Sugar in Sol.
Sugar.
CaO:
I
0.50
62.5
2
0-75
36.0
3
I .02
32-5
4
I .22
30.2
5
i-45
28.5
6
1.67
27.7
8
2 .22
27-5
10
2.77
27-5
12
3-27
27-5
14
3-85
27-5
In the second series a very much larger excess of lime was used than
in the first series. The author gives results in a subsequent paper, —
Bull. soc. chim. [3] 23, 740, 'oo, — which show that the solubility is also
affected by the condition of the calcium compound used, i.e., whether
the oxide, hydrate, or milk of lime is added to the sugar solutions.
A very exhaustive investigation of the factors which influence the solubility
of lime in sugar solutions is described by Claasen (1911).
CALCIUM IODATE 206
CALCIUM IODATE Ca(IO3)2.6H2O.
SOLUBILITY IN WATER.
(Myiius and Funk — Ber. 30, 1724. '97; W. Abh. p. t. Reichanstalt 3, 448, 'oo.)
t *
Gms.
Ca(I03)2
Mols.
Ca(I03)2 Solid
t °.
Gms.
Ca(I03)2
Mols.
Ca(I03)2
Solid
I .
per 100
Gms. Sol.
per 100 Phase.
Mols.H2O.
per 100
Gms. Sol.
per 100 Phase.
Mols. HaO.
0
0
.10
0
.0044 Ca(IO3) .6Hj
jO 21
0
•37
0
.016
Ca(I03)2.H20
10
0
•17
0
.0075
35
0
.48
O
• O2I
it
18
O
•25
0
.Oil
40
o
•52
O
023
u
30
0
.42
O
.019
45
o
•54
0
.024
it
40
0
.61
0
.027
5°
0
•59
0
.026
"
50
0
.89
0
.040
60
0
•65
O
.029
"
54
I
.04
0
.046
80
0
•79
O
•034
tt
60
I
•36
O
.063
100
o
•94
0
.042
tt
Density of solution saturated at 18° = i.oo.
CALCIUM IODIDE CaI2.
SOLUBILITY IN WATER.
(Average curve from the results of Kremers — Pogg. Ann. 103, 65, '58; Etard — Ann. chim. phys. [7]
2, 532, '94-)
«. o Cms. CaI2 per 100 f 0 Cms. CaI2 per 100 . 0 Cms. CaI2 per 100
Cms. Solution. Cms. Solution. Cms. Solution.
o 64.6 30 69 80 78
10 66. o 40 70.8 100 81
20 67.6 60 74
Density of solution saturated at 20° = 2.125.
The fusion-point curve (solubility, see footnote, p. i) is given for mixtures of
calcium iodide and iodine by Olivari (1908).
CALCIUM IODO MERCURATE.
A saturated solution of CaI2 and HgI2 in water at 15.9° was found by Duboin
(1906) to have the composition CaI2.i.3HgI2.i2.3H2O; d = 2.89 and the solid
phase in contact with the solution was CaI2.HgI2.8H2O.
CALCIUM PerlODIDE CaI4
f Data for the formation of calcium periodide in aqueous solution at 25° are
given by Herz and Bulla (1911). (See reference note under calcium perbromide,
p. 189.)
CALCIUM LACTATE Ca(C6H10O6).5H2O.
100 gms. H2O dissolve 3.1 gms. of the salt at o°, 5.4 gms. at 15° and 7.9 gms.
at 30°. (Hill and Cocking, 1912.)
CALCIUM MALATE CaC4H4O6.H2O.
SOLUBILITY OF CALCIUM MALATE IN WATER AND IN ALCOHOL.
(Partheil and Hubner, 1903.)
ioo gms. H2O dissolve 0.9214 gm, CaC4H4O6.H2O at 18°, and 0.8552 gm. at
100 gms. 95% alcohol dissolve 0.0049 gm. CaC4H4O6.H2O at 18°, and 0.00586
gm. at 25°.
207
CALCIUM MALATE
CALCIUM (Neutral) MALATE Ca(C4H4O6).3H2O.
CALCIUM (Acid) MALATE Ca(C4HBO6)2.6H2O.
CALCIUM MALONATEtCa(C3H2O4)4H2O.
SOLUBILITY OF EACH IN WATER.
(I wig and'Hecht, 1886; Cantoni and Basadonna, 1906; the malonate, Mic^ynski, 1886.)
Ca. Neutral Malate.
Cms. CaCCJfcOs) per 100
t°.
6ms.
Gms.
cc. Sol.
HzO.
Sol.
(C and B).
0
10
0.85
0.84
20
0.82
0.81
0.907
30
0.78
0.77
0.835
40
0.74
0-73
0.816
50
0.66
0.65
0.809
57
0-57
0.56
60
0.58
0.58 .
0.804
70
0.63
0.63
0-795
80
0.71
0.70
0-754
90
0.740
Ca. Acid Malate.
Cms. Ca(C4H5O5)2 per
100 Cms.
Ca. Malonate.
Water.
2
5-2
15 '
32.24
26
II
6.8
Solution.
1.77
I.48
1.96
4-94
13.09
24.29
20.64
9.91
6-37
per 100 Gms. HjO.
0.290 (0.374)
0.330 (0.419
0.365 (0.460
0.396 (0.495
0.422 (0.524
0.443 (0.544)
0.460
0.472
0.479
The results for calcium malonate given above in parentheses are by Cantoni
and Diotalevi (1905), but these authors fail to state the terms in which their
data are reported. By comparison with other papers of the series, it is prob-
able that in this case the figures refer to grams per 100 cc. saturated solution.
CALCIUM NITRATE Ca(NO3)2.4H2O.
SOLUBILITY IN WATER.
(Bassett and Taylor, 1912.)
(Silica vessels used. Constant agitation at constant temperature for two to three
days. Calcium determined by precipitation as oxalate and weighing as oxide.)
Gms.
Ca(NOs)2 Solid
per 100 Gms. Phase.
Sat. Sol.
53.55 Ca(N03)2.4HJ0
54-94
56.39
57.98
60.41
62.88
66.21
68.68
68.74
71.7
70.37
Gms.
to Ca(N03>2
per 100 Gms.
. Sat. Sol.
Solid
Phase.
— 0.4
1.4
Ice
— 1-4
4.78
"
- 1-9
6-53
"
- 3-05
IO
"
— 4-15
12.98
"
-15-7
33-13
"
-21.7
38.7
"
-28.7
*
-26.7
43-37 C*
t(NOs)j.4
— IO
47-31
"
o
50.50
M
5
Si-97
1C
10
IS
20
25
30
35
40
42.4
42.4
42.7
42-45
40
t m. pt.
Gms.
to
Ca(NO3)2 Solid
.
per 100 Gms. Phase.
Sat. Sol.
45
7L45
Ca(N03)i.3H,0
50
73-79
"
Si
74-73
«
49
77 -4£
Ca(NOj)«.2H.O
5i
78.05
"
£
78.16
78.2
Ca(NOi)i
100
78.43
"
125
78.57
•
147.
5 78.8
"
151
79
"
Eutectic.
SOLUBILITY OF THE UNSTABLE CALCIUM NITRATE TETRAHYDRATE /3 IN WATER.
(Results supplementary to the above.)
(Taylor and Henderson, 1915.)
Gms. Ca(NO3)2
t°.
per 100 Gms.
Sat. Sol.
o
50.17
22.2
56.88
25
57-9°
30
60. 16
30
6i.57
34
63.66
35
62.88
38
64.34
Solid Phase.
aCa(N03)j.4H20
/3Ca(NOa)2.4H2O
Gms. Ca(NO..)a
t8.
per zoo Gms.
Sat. Sol.
38
66.65 ,
39
67-93
39.6 (m. pt.)
69.50
39 (reflex pt.)
75-34
40
66.22 <
42 . 7 (m. pt.)
69.50
42.4 (reflex pt.)
71.70
25
77.30
Solid Phase.
0Ca(NOs)«.4H»O
Ca(NOi)«
CALCIUM NITRATE
208
SOLUBILITY OF CALCIUM NITRATE IN AQUEOUS SOLUTIONS OF CALCIUM
THIOSULFATE AT 9° AND AT 25° AND VICE VERSA.
(Kremann and Rodemund, 1914.)
Results at 9°.
Results
at 25°.
Gms. per ioo Gms. Sat. Sol.
Gms. per ioo Gms. Sat. Sol.
Solid Phase.
'Ca(NOa)«.
CaS203. '
'Ca(NO3)2.
CaS2O3.
46.02
5.46 Ca(NOs)2.4H:O
54-03
4.27
Ca(N03)2.4HiO
45-68
6. 8 1 " •fCaSiOs.GHzC
> 50.25
9-IO
"
27.92
10.46 CaS^.GHzO
45-92
13
" +CaS2Oa.6HK)
10.49
22. 8l
42-93
I3-83
CaSzOs-GHW)
29-33
32.01
17.09
"
I9-5I
23.78
"
8.15
SOLUBILITY OF CALCIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AT 9° AND AT 25° AND VICE VERSA.
(Kremann and Rodemund, 1914.)
Results at 9°.
Gms. per 100 Gms. Sat. Sol.
Ca(NO3)2. NaNOa. '
47.51 9.51
46.08 12.56
26.67 23.32
11.76 34.26
Solid Phase.
Ca(N03)2.4H20
" +NaN03
NaNO«
Results at 25'
Gms. per 100 Gms. Sat, Sol.
Ca(NO3)2.
NaNO3."
54.58
7-25
53-22
10.70
52-73
12.08
52.40
11.88
37-31
19.48
26.91
24.98
I4.6l
36.12
Solid Phase.
Ca(NOi)2.4H20
" +NaNO,
NaNOi
These authors also give the complete solubility relations of the reciprocal
salt pairs, Ca(NO3)2 + Na^Oj ±=> 2NaNO3 + CaS2O3 at 9° and 25°.
SOLUBILITY OF CALCIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT 25°.
(Bassett and Taylor, 1912.)
(The mixtures were shaken intermittently, by hand, during quite long periods;
one week was allowed between duplicate determinations.)
Gms. per 100 Gms. Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol. Solid Phase. Sat. Sol. Solid Phase. _ Sat. Sol. Solid Phase.
Ca(NOi)i. HN03. Ca(NO3)2. HNO3. Ca(NO3)2. HNO3.
57 . 98 O Ca(N03)j.4H20 3 2 . 84 32 . 63 Ca(NO3)2.4H2O 9 . 34 65 . 69 Ca(NO3)2.2HjO
54.82 3.33
52.96 5.87
51.58 7.21
47.82 11.27
45-59 I3-7I
40.70 19.65
38.17 22.80
34.46 28.81
Freezing-point data for the Ternary System Ca(NO3)2-r-KNO3 + NaNOs are
given by Menzies and Dutt, 1911.
SOLUBILITY OF CALCIUM NITRATE IN SEVERAL ORGANIC SOLVENTS.
32.50
33-52
"
8.52
67.20
33-44
35.63
Ca(NO3)2.3HjO
5-o6
71.12 Ca(NOi)2
29.05
41.66
"
2-53
74-77
27-79
45-70
"
1.05
78.56
31.09
40.56
Ca(NOa)«.2H,0
0-54
80.83
26.07
45-70
ft
0.36
85-83
17.41
55-48
"
O.OI
90.90
12.25
62.05
"
o
96.86
Solvent.
Gms. Ca(NO3)j per 100 Gms.
N Sat. Solution.
Methyl Alcohol
Propyl "
i Butyl "
Amyl
Acetone
Methyl Acetate
25
25
25
25
25
18
65.$
36.5
25
13-3
58.5
4i
Authority.
(D'Ans and Siegler, 1913.)
(d sat . sol. =1.313) (Naumann, 1 909.) j
209
CALCIUM NITRATE
SOLUBILITY OF CALCIUM NITRATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL
AT 25°. (D'Ans and Siegler, 1913.)
Gms. per too Gms. Sat. Sol.
C2HsOH.
Ca(N03)2.
O
57-5
8.1
55-2
14.1
52-9
22.3
50.2
29.4
49
31.2
52
29-5
56.2
27.8
60
26.5
62.3
0
82.5
5-8
77
Solid Phase.
Gms. per 100 Gms. Sat. Sol.
Ca(N03)2.4H20
" +Ca(NOi),
Ca(NOa)j unstable
CALCIUM NITRITE Ca(NO2)2.4H2O.
SOLUBILITY IN WATER.
CzHaOH.
Ca(NO.-)2.
15-2
69.52
20-4
66.08
35-9
57-7
41.8
51-4
27-39
61.96
28.5
61.15
29.6
60.3
60.2
38.6
54-6
41.9
42.5
50-97
35-8
55-3
Solid Phase.
Ca(NOs)2 unstable
CaCNOs)* stable
Ca(NOs)2.2C2H60H
(Oswald, 1914.)
Solid Phase.
- 4
~ 9-3
-12. 5
-14-5
-17-5
^ 9-5
o
16
16.7
25-5
29-5
32
35
36.2
38-3
Ice
[r Solid Phase.
CaCNO^^HzO
+Ca(N02)2.4H20
42
44
54
64
70
73
+Ca(NOJ)J.2H10
43
51.8
53-5
55-2
58
60
61
71
An aqueous solution simultaneously saturated with calcium nitrite and silver
nitrite, contains 92.4 gms. Ca(NO2)2 + 11.2 gms. AgNO2 per 100 gms. H2O at 14°.
(Oswald, 1914.)
100 cc. sat. solution of calcium nitrite in 90 % alcohorcontain 39 gms. Ca(NO2)2.
H2O at 20°.
100 cc. sat. solution of calcium nitrite in absolute alcohol contain i.i gms.
Ca(NO2)2.H2O at 20°. (Vogel, 1903.)
CALCIUM OLEATE (C^O-OCa.
One liter water dissolves about o. i gm. calcium oleate at t°not stated. (Fahrion, 1916.)
100 gms. glycerol (of d = 1.114) dissolve 1.18 gms. calciumoleate at t° not stated.
(Asselin, 1873.)
CALCIUM OXALATE Ca(COO)2.H2O.
SOLUBILITY IN WATER, BY ELECTROLYTIC CONDUCTIVITY METHOD.
(Holleman, Kohlrausch, and Rose, 1893; Richards, McCaffrey, and Bisbee, 1901.)
*o Gms. CaC2O4 per
Liter of Solution.
13 0.0067 (H)
08. 0.0056 (K and R)
24 0.0080 (H)
«.<> Gms. CaC2O4 per
Liter of Solution.
25 0.0068 (R, McC and B)
50 0.0095
95 0.0140
SOLUBILITY OF CALCIUM OXALATE IN AQUEOUS SOLUTIONS OF ACETIC ACID AT
26°-27°. (Herz and Muhs, 1903.)
Normality of
Acetic Acid.
O
0.58
2.89
5-79
G. CH3COOH
per 100 cc. Sol.
0-00
17-34
34-74
Residue from 50.053
cc. Solution.
0.0017
0.0048
0-0058
0.0064
The residues were dried at 70° C.
CALCIUM OXALATE 210
SOLUBILITY OF CALCIUM OXALATE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID AT 25°.
(Henderson and Taylor, 1916.)
NonnaUtyofHCl. ^S^ Normality of HC1.
o 0.009 0.500 2.638
0.125 0.717 0.625 3.319
0.250 1.359 0.750 3.922
0.375 2.019 I 5.210
These authors also give data showing the effect of increasing amounts of KC1
and KNO3 upon the solubility of calcium oxalate in 0.5 normal HC1 at 25°, and
also of the effect of increasing amounts of potassium trichloracetic acid upon the
solubility in 0.5 normal trichloracetic acid, and of increasing amounts of potas-
sium monochloracetic acid upon the solubility of calcium oxalate in 0.5 normal
monochloracetic acid.
SOLUBILITY OF CALCIUM OXALATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE
AND OF SODIUM PHOSPHATE.
(Gerard, 1901.)
Salt in Aq. Cms. Salt to Cms. CaCzOt Salt in Aq. Cms. Salt to Cms. CaCzCU
Solution. per Liter.. per Liter. Solution. per Liter. per Liter.
NaCl i 25 0.0075 NaCl 25 37 0.0414
5 25 0.0188 Na2H(P04)2 4.8 15 0.016
10 25 0.0255 4.8 37 0.033
25 ,25 0.0291
One liter 45% ethyl alcohol dissolves 0.000525 gm. calcium oxalate, temp, not
Stated. (Gueiin, 1912.)
CALCIUM OXIDE CaO.
100 gms. molten CaCl2 dissolve 16.2 gm. CaO at about 910°.
(Arndt and Loewenstein, 1909.)
Data for the systems, CaO -f- MgO and for CaO + A12O3 + MgO are given by
Rankin and Merwin (1916); for CaO + A12O3 + SiO2 by Rankin and Wright
(1915); for CaO + Fe2O3 by Sosman and Merwin (1916); and for CaO + MgO
+ SiO2 by Bowen (1914).
Data for the system CaO + C + CaC2 + CO are given by Thompson (1910).
CALCIUM PHOSPHATE (Tribasic) Ca3(PO4)2.
SOLUBILITY IN WATER.
The determinations of the solubility of this salt in water, as stated in the
literature, are found to vary within rather wide limits, due, no doubt, to the
fact that so-called tribasic calcium phosphate is apparently a solid solution of
the dibasic salt and calcium oxide, and therefore analyses of individual samples
may show an excess of either lime or phosphoric acid. When placed in contact
with water, more PO4 ions enter solution than Ca ions, the resulting solution
being acid in reaction and the solid phase richer in lime than it was, previous to
being added to the water. For material having a composition approximating
closely that represented by the formula Ca3(PO4)2 the amount which is dissolved
by CO2 free water at the ordinary temperature, as calculated from the calcium
determination, is o.oi to o.io gram per liter, depending upon the conditions of
the experiment. Water saturated with CO2 dissolves 0.15 to 0.30 gram per
liter.
A list of references to papers on this subject is given by Cameron and Hurst —
J. Am. Chem. Soc., 26, 903, 1904; see also Cameron and Bell, Ibid., 27, 1512, 1905.
211
CALCIUM PHOSPHATE
CALCIUM PHOSPHATE (Dibasic) CaHPO4.2HaO.
SOLUBILITY IN WATER.
(Cameron and Seidell — J. Am. Chem. Soc. 26, 1460, '04; see also Rindell — Compt. rend. 134, iza, 'oaj
Magnanini — Gazz. chim. ital. 31, II, 544, *oi.)
i liter of CO2 free water dissolves 0.136 gram CaHPO4 at 25°.
i liter of water sat. with CO2 dissolves 0.561 gram CaHPO4 at 25°.
SOLUBILITY OF Di CALCIUM PHOSPHATE AND OP MONO CALCIUM PHOS-
PHATE IN AQUEOUS SOLUTIONS OF PHOSPHORIC ACID AT 25°.
(Cameron and Seidell — J. Am. Chem. Soc. 27, 1508, '05; Causse — Compt. rend. 114, 414, '92.)
Grams per Liter of
Solution.
Gms. per Liter
Calc. from CaO Found.
PaO5 per Liter
in Excess of e rj t>v.
that combined Sohd Phase-
CaO.
P205.
with Ca.
I .71
4.69
4-J5
CaHP04
2-53
CaHP04.2ILO
"•57
36.14
28.05
"
21.5
u
23 -31
75-95
56-53
tt
46-45
ft
39.81
139.6
97-Qi
"
89.0
tt
49.76
191.0
120.7
tt
128.0
tf
59-40
234.6
144.1
u
159-4
tt
70-31
279.7
170.6
tt
190.7
tt
77.00
317.0
( 174.2
(321.3
CaHPO, or
CaH4(P04)2
226.0
122.2
CaHPO4.2H
CaH4(PO )r!
.0+
E^O
72.30
35J-9
301.6
CaH4(P04)2
169.0
CaH4(P04)2.:
Hp
69-33
361.1
289-3
a
186.1
M
59 98
419.7
250.2
tt
267.9
tl
53-59
45J-7
223-7
ft
316.1
tt
44-52
505-8
185.8
tt
393-1
ft
39-89
538.3
166.4
tt
437-4
tt
Density of the solution in contact with both salts at 25° = 1.29.
SOLUBILITY OF CALCIUM PHOSPHATES IN AQUEOUS SOLUTIONS OF PHOSPHORIC
ACID AT DIFFERENT TEMPERATURES.
(Bassett, Jr., 1908, 1917.)
Results at 25°. Results at 40°. Results at 50.7°.
Gms. per 100
Gms. Sat. Sol. Solid Phase.
Gms. per 100
Gms. Sat. Sol.
Solid Phase.
Gms. F
Gms. S
S- too
. Sol.
Solid Phase.
CaO.
P206.
CaO.
P2O5.
CaO.
p2o6:
3.088
36.11 CaHiPjjOs.HiO
1.768
42.42
CaH*P208.H20
0.336
62.01
CaH*P208+
4.908
28.34
3.584
36.79
"
CaHiPjOg-aO
5.809
24.20
+CaHPO*
5-755
27.25
" +CaHPO*
0.635
58.08
CaH*PjO».H2O
5.523
22.90Ca
HPO*
4.813
21.67
CaHPO*
1.428
50.25
"
4-499
17.55
3.810
16.35
2.974
41.92
"
2.638
9.100
2.536
9-905
4.880
33.18
•«
1.878
6.049
1.847
6.979
5.725
29.61
" +CaHPO*
0.826
2.387
1.267
4.397
3.507
15.48
CaHPO*
0.165
0.417 ( ' CaHPO*.
0.576
1.819
2.328
9.465
»
0.07
0.166 1 2H2O
0.156
0.426
"
I.563
6.157
»
O.o6
0.140
0.0592
0.158
"
0.692
2.281
"
0.05
0.118 "
0.0508
0.128
Ca3P208.HjO
0.0596
0.1527
CaHPO*.aHjO
0.04
0.093
0.0098
0.0262
"
0.0514
0.1331
CaaPjOs-HjO
0.03
0.070! .
0.0709
trace
Ca*P209.4H20
0.0351
0.0942
"
0.02
0.047 f r 'TXPO^'TT r\
1 0.0814
"
"
0.0106
0.0309
"
O.OI
0.023J a 4'2 2
0.0840
"
"
0.0007
0.0007
"
In the case of most of the solutions 7-15 weeks constant agitation was allowed
for attainment of equilibrium. For the last seven results at 25°, 18 months
were required. Cerasine bottles were used in these cases. The solid phases
were determined by analysis. The quintuple points were found by dilatometer
experiments at 36°, 21° and 152°. (See next page.)
CALCIUM PHOSPHATES 212
SOLUBILITY OF CALCIUM PHOSPHATES IN AQUEOUS SOLUTIONS OF PHOSPHORIC
ACID AT TEMPERATURES ABOVE 100°.
(Bassett, Jr., 1908.)
Cms. per 100 Cms Sat. Sol.
*° -Caa - ' - PloT- SohdPhase,
100 2.503 53-71 CaH4P208+CaH4P208.H20
1 15 b. pt. 5 . 623 43 . 60 CaH4P208.H20+CaHP04
132 " 4-327 53-43 CaH4P208+CaH4P208.H20
169 " 4-489 63.95 CaH*P208
The quintuple points for the system determined by dilatometer experiments
are as follows:
5.60 53 ; CaH4P208+CaH4P208H20+CaHP04
152
21
36
5.81
0.0514
23.5
0.14
CaH4P2Os.H20+CaHP04+CaHP04.2H20
CaHPO4+CaHP04.2H2O+Ca3P2Os.H2O
Salt in Aq. Solvent.
Gms. Salt
For additional data on the solubility of calcium phosphates in water, see
Cameron and Bell, 1905 and 1910.
Data for the four component system, lime, phosphoric acid, sulfuric acid and
water, the essential constituents of "superphosphates," are given by Cameron
and Bell (1906).
One liter of aqueous 0.005 n potassium bitartrate solution sat. with calcium
phosphate, contains 0.08 gm. Ca and 0.181 gm. HaPO4 at 25°. (Magnanini, 1901.)
SOLUBILITY OF CALCIUM PHOSPHATE IN AQUEOUS SALT SOLUTIONS UNDER 2
ATMOSPHERES PRESSURE OF CO2 AT 14°.
(Ehlert and Hempel, 1912.)
Gm
Salt in Aq. Solution.
Solventi
70.95 1.777
cone.
K2SO4 74-5
cone.
NaCl 50
" cone.
NaNOs 72.7
Cone.
Na2SO4.ioH2O 137.7
conc-
per
Gms.
Water
NH4C1
45-74
a
cone.
(NH4)2S04
56.5
«
cone.
MgCl2.6H2O
86.9
11
cone.
MgS04.7H20
105.3
u
cone.
MgCl2.KC1.6H2O
79.2
(i
cone.
MgSO4.K2SO4.MgCl2.6H2O
2.491
4.904
4.765
1.321
0.641
1.583
0.864
2.491
3-227
Gms. Salt
per ioo
Gms. HaO.
0.228
I-37I
1.293
2.413
5-885
1.287
2.892
1.9728
3.6001
1-577
I.I54
Data for the solubility of calcium phosphate in aqueous saturated solutions of
carbon dioxide containing ammonia are given by Foster and Neville, 1910.
CALCIUM PELARGONATE (Nonate) Ca[CH3(CH2)7 COO]2.H2O.
CALCIUM PROPIONATE Ca(CH3.CH2COO)2.H2O.
SOLUBILITY OF EACH IN WATER.
(Lumsden, 1902; Krasnicki, 1887.)
Calcium Pelargonate.
Gms.
t". Ca[CH3(CH2)7COOla
per ioo Gms. H-iO.
0
20
40
00
80
90
ioo
O.l6
0. 14
0.13
0.12
0.15
0.18
0.26
Calcium Propionate.
Gms. Ca(CH3.CH2COO)2 per ioo Gms.
Water.
42.8O
39-85
38.45
38.25
39.85
42.15
48.44
Solution.
29.97
28.48
27.76
27.67
28.48
29.66
32.63
213 CALCIUM SALICTLATE
CALCIUM SALICYLATE Ca(C6H4.OHCOO)2.3H2O.
100 grams of the saturated aqueous solution contain 2.29 grams of the an-
hydrous salt at 15° find 35.75 grams at IOO°. (Tarugi and Checchi, 1901.)
CALCIUM SELENATE CaScO4.
SOLUBILITY IN WATER
(Etard — Ann. chim. phys. [7] 2, 532, '94.)
t°. -i°. +5°. 20°. 37*. 67°.
Gms. per ioo gms. sol. 7.4 7.3 7.6 6.8 5.1
The accuracy of these results appears questionable.
CALCIUM SILICATE CaSiO3.
SOLUBILITY IN WATER AND IN AQUEOUS SUGAR SOLUTIONS AT 17°.
(Weisberg — Bull. soc. chim. [3] 15, 1097, '96.)
The sample of calcium silicate was air dried.
Grams per ioo cc. Saturated Solution.
Solvent. At^i?0. After Boiling and Filtering Hot.
CaO(det-) ' CaSiO3(calc.) CaO(det.) CaSiOs(calc.)
Water 0.0046 0.0095
i o% sugar sol. 0.0065 0.0135 0.0094 0.0195
20% sugar sol. 0-0076 0-0157 0-0120 0-0249
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES OF CALCIUM SILICATE AND OTHER COMPOUNDS.
CaSiOs + CaS (Lebedew, 1911.)
-j- CaTiOs (Smolensky, 1911-12.)
-j- Li2Sip3 (Wallace, 1909.)
+ MgSiO3 (Allen and White, 1911; Ginsberg, 1906.)
+ MnSiO3 (Ginsberg, 1908, 1909.)
+ Na2SiO3 (Wallace, 1909; Kultascheff, 1903.)
CALCIUM SUCCINATE Ca(C2H202)2.
CALCIUM (Iso) SUCCINATE CaCH3.CHC2O4.H2O.
SOLUBILITY OF EACH IN WATER.
(Miczynski, 1886.)
Calcium Succinate. Calcium Iso Succinate.
Gms. w Gms. Gms. Gms.
to Ca(C2H202)s to Ca(C2H2Oi)2 t» Ca(CjH«Oi)i t» Ca(C2H2O2)j
per ioo Gms. ' per ioo Gms. ' per ioo Gms. per ioo Gms.
H20. HzO. H.O. H£>.
o 1.127 50 1.029 o 0.522 50 0.440
10 1.220 60 0.894 10 0.524 60 0.396
2O 1.276 70 0.770 2O 0.517 7O 0.342
40 1.177 80 0.657 4° °-475 8° 0.279
ioo cc. H2O dissolve 1.424 gms. CaC4H4O4.H2O at 18° and 1.436 gms. at 25°
(Partheil and Hubner, 1903.)
ioo gms. H2O dissolve 1.28 gms. CaC4H4O4 at 15° and 0.66 gms. at 100°.
(Tarugi and Checchi, 1901.)
Results for calcium succinate in water, varying considerably from the above and
indicating an increase of solubility with temperature, are given by Cantoni and
Diotalevi (1905) but the terms used for expressing the results are not stated.
ioo cc. 95% alcohol dissolve 0.00136 gm. CaC4H4O4.H2O at 18° and 0.00136 gm.
at 25°. (Parheil and Hubner, 1903.)
CALCIUM SULFATB 214
CALCIUM SULFATE CaSO4.2H20.
SOLUBILITY IN WATER.
(Hulett and Allen, 1902; for references to other determinations see Hulett and Allen, also Euler, 1904.
For data by the electrolytic conductivity method, see Holleman, Kohlrausch and Rose, 1893, 1908.)
Gms. CaSO*
t°. per 100 cc.
Solution.
Millimols
per Liter.
Density of
Solutions.
Gms. CaSO4
t°. per loo cc.
Solution.
Millimols
per Liter.
Density of
Solutions
O
o,
1759
12
.926
I.OOI97
40
o.
2097
15
•413
0.99439
10
o,
,1928
14
.177
I.OOI73
55
o.
2009
14
.765
0.98796
18
0.
,2016
14
.817
I . OOO59
65-3
0.
1932
14
.2OO
0.98256
25
0.
,2080
15
.235
0.99911
75
o.
1847
13
•575
0.97772
30
o,
,2090
15
.361
0.99789
IOO
o.
1619
II
.900
35
o,
,2096
15
•4°S
0.99612
107
II
•390
SOLUBILITY OF CALCIUM SULFATE ANHYDRITE AND OF SOLUBLE ANHYDRITE
IN WATER. (Melcher, 1910.)
to MiUimols PCr GmS'LiteSr°4 *** Solid Phase'
loo 11.65 1-586 CaSO4.2H20
loo 11.4 i .55 2 Soluble anhydrite
100 4.6 0.626 Anhydrite
• 156 3.2 0.436 Soluble anhydrite
156 1.35 0.184 Anhydrite
218 °-35 - 0.048 "
Data' for the solubility.'of calcium sulfate in sea water are given by Manuelli, 1916.
SOLUBILITY OF CALCIUM SULFATE IN .AQUEOUS^SOLUTIONS OF AMMONIUM
ACETATE AT 25°. (Harden, 1916.)
Cms. CH3COONH4 per , Cms. CaSO4 per
loo Gms. Solution. 100' Gms. Sat. Solution.
o I 0.2085
2.13 1.005 0.454
5.34 I. 012 0.752
10.68 1.024 1.146
21-37 1-045 1.755
SOLUBILITY OP CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OP HYDRO-
CHLORIC, NITRIC, CHLOR ACETIC, AND FORMIC ACIDS.
(Banthisch — J. pr. Chem. 29, 52, '84; Lunge — J. Soc. Chem. Ind. 4, 32, '85.)
In Hydrochloric. In Nitric. In Chlor Acetic. In Formic.
Grams Acid Grams CaSO4 per
per TOO cc. i°o cc. Sol.
Gms. CaSO4 per
loo cc. Solution
Gms. CaSO4 per
IOO CC. Sol.
Gms. CaSO4 per
loo cc. Soi.
Solution.
at 25°.
at
I026.
at 25°.
at 25°.
at 25°.
0
O
.208
o,
,160
O
.208
O.2O8
0.208
I
0
.72
I.
38
0
•56
2
I
.02
a.
38
0
.82
3
I
•25
3
20
I
• O2
4
I
• 42
3.;
64
I
.20
0.22
0.24
6
I
•65
4'
1 6^
I
.48
. . .
8
I
•74
.
I
.70
10
.
I
.84
0.25
12
.
. .
,
. .
I
.08
. . .
. . .
Data for the solubility of mixtures of CaSO4(NH4)2 SO4.H2O + (NH4)2SO4 and of
CaSp4(NH4)2SO4.4H2O + CaSO4.2H2O at various temperatures between 3° and 100°
are given by Barre, 1909 and 1911. Additional data for this system, including re-
sults for the pentacalcium salt, (NH4)2Ca6(SO4)6.H2O, are given by D'Ans, 1909.
215
CALCIUM SULFATE
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF AMMONIUM
SALTS.
(In NH4C1 and NH4NO3, Cameron and Brown — J. Physic. Chem. g, 210, '05 ; In (NH4)2SO4 at 25°,
Sullivan — J. Am. Chem. Soc. 27, 529, '05; In (NKO-jSCu at 50°, Bell and Tabor — J. Physic. Chem. 10,
InNH4Cl InNH4NO3 In NH4C1 In NH4NO3
at 25°.
at 25°.
at 25°.
at 25°.
Gms. Ammo-
nium Salt
G.CaSO4
Dissolved
G. CaS04
Dissolved
Gms. Ammo-
nium Salt
G. CaS04
Dissolved
G. CaSO4
Dissolved
per Liter.
per Liter.
per Liter
per Liter.
per Liter.
per Liter.
O
2.08
2.08
300
IO.IO
10.80
2O
5-oo
3-70
375
7-40
40
7-00
5-10
400
11.40
60
8.00
6.05
600
12.15
80
8.50
7-00
800
12 .IO
IOO
9-10
7-65
1000
•
ii. 81
J5o
10.30
8.88
1400
10-02
200
10.85
9-85
sat.
7-55
In
(NH4)2S04at25°.
In (NH^SO, at
5o°.
Grams per Liter Sol. Wt. of ioo CC.
Grams per
Liter Sol.
Sp. Gr.
(NH^SO
4. CaS04.
Sat. Sol.
'(NH4)2S04.
CaSO4. ' of Solutions.
O
2.08
99.91
0
2.168
. . .
0.129
2.O4
99.91
I5-65
1.609
1.0026
0.258
1.99
99.92
30-67
1-750
I.OII3
0.821
1.81
99-95
91 .6
2.542
1.0440
1.643
1.66
99.99
160.4
3.402
.0819
3.287
1.54
100.10
221.6
4.068
.II08
6-575
1.44
100.34
340.6
5.084
•1653
1.46
100.82
416.5
5-354
.1964
26.30
1.62
101.76
428.4
4.632
.2043
84.9
2.33
105.34
530.8
2 .152
•2437
169.8
3-33
110.32
566
1. 08
1.2508
339-6
4-50
119.15
566.7
0
I.25IO
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF CALCIUM SALTS
AT 25
(Cameron and Seidell — J. Physic. Chem, 5. 643. 'or, Seidell and Smith — Ibid. 8, 493, '04; Cameron
and Bell — J. Am. Chem. Soc. 28, 1220, '06.)
In Calcium
Chloride.
Grams per Liter Sol.
In Calcium
Nitrate.
Gms. per Liter Sol.
Wt.of
In Calcium Hydroxide and
vice versa.
Gms. per Liter Sol. Solid
" CaCl2.
CaS04. "
Ca(N03)2.
CaS04.
x
cc. Sol.
Ca07~
CaS04.
Phase.
o.oo
2
.06
o.o
2.08
0
•998
0
.0
2
.126
CaS04.2H,0
7-49
'z
.24
25 -
1.24
:z
.014
0
.062
2
.030
«
II .96
I
.18
50
1.20
z
.032
O
.176
I
.918
a
25-77
Z
.10
IOO
I.I3
z
.067
O
•349
Z,
853
tt
32-05
I
.08
200
o-93
z
•137
O
.61
z
.722
it
51 .53
I
.02
300
0.76
z
.204
o
•939
I,
634
"
97.02
0
.84
400
o-57
i
.265
I
.222
I.
588
1 CaS04.2H2O+
! Ca(OH)3
192.71
o
•47
500
0.40
i
.328
I
.242
z
.214
Ca(OH),
280.30
0
.20
544
o-35
i
•352
I
.150
0
.666
"
367-85
0
•03
I
.166
0
• oo
M
CALCIUM SULFATE
216
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF COPPER SULFATE
AT 25°.
(Bell and Taber, 1907.)
Cms, per Liter Sat. Sol.
dK Sat. Sol.
Gms. per Liter Sat. Sol.
CuS04.
CaSOi.
U23 OO.I. OU1.
CuSO4.
CaSOi.
an oai. aoi.
I.I44 -
2.068
1.002
39-407
I.7I8
I.04I
3-564
.986
I.OO5
49.382
1.744
I.05I
6.048
•944
I .OO7
58.880
1.782
1.061
7.279
.858
1.009
97-950
I-93I
1.098
14.814
.760
1.016
146.725
2.048
1.146
19.729
•736
1. 021
I96.O2I
2.076
1.192
29-543
.688
1.030
224.916
2.088
i. 218
SOLUBILITY OF MIXTURES OF CALCIUM SULFATE AND CAESIUM SULFATE IN
WATER.
(D'Ans, 1908.)
te.
25
60
Mols.CsjS04.CaS04
per 1000 Gms.
Sat. Sol.
0.667
0.607
Gms. Cs2SO4.CaS04
per 1000 Gms.
Sat. Sol
352
320
Solid Phase.
Dicalcium Sulfate + Gypsum
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF MAGNESIUM
CHLORIDE AND OF MAGNESIUM NITRATE AT 25°.
(Cameron, Seidell, and Smith.)
In Magnesium Chloride. In Magnesium Nitrate.
Grams per Liter of Sat. Solution.
MgCl2.
CaS04.
HzO."
O
2.08
997-9
8.50
4.26
996.5
I9.I8
5-69
994-5
46.64
7-59
989.1
121.38
8.62
972.2
206.98
6-57
949-9
337
2.77
908.7
441.1
i-39
878.6
warns per
L,iter solution.
Wt. of i cc.
Mg(NOs)2.
CaS04.
Solution.
0
2.08
0.9981
25
5-77
1.0205
50
7.88
I .0398
100
9.92
1.0786
200
13-34
1.1498
300
14
I.2I90
4OO
14.68
I.282I
514
15.04
1-3553
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF MAGNESIUM
SULFATE AT 25°.
(Cameron and Bell, 19063.)
Grams per Lit
er Solution. 5
p. Gr. of
tions at f$ °.
MgSO4.
CaS04." Sok
0
2.046
.0032
3-20
1.620
•0055
6-39
1.507
.0090
10.64
I.47I
.OIl8
21.36
1.478
.O226
42.68
1-558
.0419
64.14
1. 608
.0626
85.67
1.617
•0833
128.28
1.627
.1190
Grams per Liter Solution. J
p. Gr. of
itions at §f °
MgS04.
CaS04. *>«
149.67
1-597 1
•1377
165.7
1-549 3
.1479
I7I.2
1.474
.1537
198.8
i .422
.1813
232.1
1.254
.2095
265.6
1.070
.2382
298
0.860 :
.2624
330.6
0.647 <J
.2877
355
0.501 ,3
•3023 .
217
CALCIUM SULFATE
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF PHOSPHORIC
ACID AT 25°.
(Taber, 1906.)
Gms. per Liter.
Sp. Gr. of
Gms. per Liter.
Sp. Gr. of
0
5
21.4
46.3
105-3
SOLUBILITY OF
Grams HzSO4
per Liter of
Solution.
CaS04." Solutions at 2f . Pj(
2.126 0.9991 145
3.143 .002 205
3-734 -007 311
4.456 .016 395
5.760 .035 494
7.318 .075
CALCIUM SULFATE IN AQUEOUS S
(Cameron and Breazeale, 19
Results at 25°.
)s.
•I
j
..6
>OLUT
33.)
Resu
Gm
pe
CaS04. ' Solutions at §|.
7.920 1.106
8.383 1.145
7.965 I. 221
6.848 1.280
5.572 1.344
IONS OF SULFURIC ACID.
Its at 35°. Results at 43°.
s. CaSO4 Gms. CaSO4
r Liter. per Liter.
Gms. CaSO4
per Liter.
Wt. of
Sol
I CC.
O
• 00
2
.126
0
.9991
grams
. . .
2
•145
O
.48
2
.128
I
.0025
tt
2
.209
2
•236
4
.87
2
.144
I
.OO26
(i
2
•451
2
•456
8
.11
2
.203
I
.0051
a
2
.760
16
.22
2
.382
I
.0098
n
3
.116
48
.67
2
.727
I
.0302
tt
3
•397
3
.843
75
.00
2
.841
I
•0435
tt
4
.146
97
•35
2
•779
I
•0756
(I
3
.606
. . .
146
• 01
2
•571
t(
3
•150
4
•139
194
•70
2
•3*3
I
•1134
ft
3
•551
243
•35
I
.901
I
.1418
tt
• • «
2
•959
292
.02
I
•541
I
.1681
It
• ••
2
.481
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE, BROMIDE, AND IODIDE AT 21°.
(Ditte, 1898.)
In KC1 Solutions. In KBr Solutions. In KI Solutions
Grams of the
Potassium Salt
per Liter.
Gms. CaSO4
per Liter.
Gms. CaSO4
per Liter.
Gms. CaSO4
per Liter.
0
2.05
2.05
2.05
10
3-6
3-i
2.8
20
4-5
3-6
32
40
5-8
4-5
3-9
60
6.6
5-2
4-5
80
7-2
5-9
4-85
100
7-5
6-3
5-1
I25
double salt
6-7
5-45
150
...
7.0
5-8
20O
. . .
7-3
5-95
250
. « «
double salt
6.00
300
double salt
CALCIUM SULFATE 218
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM
NITRATE AND OF POTASSIUM SULFATE AT 25°.
(Seidell and Smith, 1904; Cameron and Breazeale, 1904.)
In Potassium Nitrate. In Potassium Sulphate.
Cms. per Liter _, Cms. per Liter
SohTtion. Wt.of.icc. Solution. Wt. of i cc.
KNOaT CaSOi. fc2SO4. ' CaSO,
o.o 2.08 0.9981 o.o 2.08 0.9981
12.5 3.28 1.0081 4.88 I. 60 1.0036
25.0 4.08 1.0154 5.09 1.56 1.0038
50.0 5.26 1.0321 9.85 1.45 1.0075
ioo. o 6.86 1.0625 19.57 1.49 1.0151
150 7.91 1.0924 28.35 1.55 1.0229
200 8.69 I.I224 30.66 1.57 1.0236
260 syngenite 1.1539 32-47 J-S8*
* Solid phase syngenite. Results for the solubility of syngenite in solutions of potassium sulphate are
also given in the original paper.
Data for the solubility of syngenite, K2Ca(SO4)2.H2O, and of potassium pentacal-
cium sulfate, K2Ca5(SO4)6.H2O, in water at various temperatures, are given by
D'Ans (1909). This author also gives results for the effect of the following salts
upon the concentration of the boundary solution for gypsum-potassium syn-
genite at 25°: KC1, KBr, KI, KC1O3, KC1O4, KNO3, CH3COOK, KOH, K4Fe(CN),
K3Fe(CN)6, NaCl, Nal, NaNOs, CH3COONa, HC1, HNO3, H3PO4f CH3COOH,
H2SO4, Ag2SO4 and cane sugar.
Data for the solubility of mixtures of CaSO4.K2SO4.H2O + CaSO4.2H20 and
CaSO4.K2SO4.H2O + K2SO4 in^water at temperatures between o° and 99°, are
given by Barre (1909, 1911).
Data for mixtures of gypsum-rubidium syngenite and of dicalcium salt-syn-
genite, at temperatures between o° and 40°, are given by D'Ans (1909).
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 26°.
(Cameron, 1901; also Orloff, 1902; Cloez, 1903; d'Anselme, 1903.)
Grams per ioo cc. Solution. \\rt. of i cc. Grams per ioo cc. Solution. \yt. of i cc.
' NaCl. CaSOT Solution. ' NaCl. CaSOT Solution.
O 0.2I2I 0.9998 17.650 0.712 1.1196
9.115 0.666 1.0644 22.876 0.679 1.1488
14.399 0.718 1.0981 26.417 0.650 1.1707
14.834 0.716 I.IOI2 32.049 0.572 1.2034
SOLUBILITY OF MIXTURES OF CALCIUM SULFATE AND CALCIUM CARBONATE IN
AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AT 23°.
(Cameron and Seidell, 1901 a.)
Grams per Liter Solution. Grams per Liter Solution.
NaCl. Ca(HC03)2. CaSCh. ' NaCl. Ca(HCO3)2. CaSO?.
o 0.060 1.930 79.52 0.060 6.424
3.63 0.072 2.72O 121.90 0.056 5.272
11.49 0.089 3.446 I93.8O 0.048 4.786
39.62 o.ioi 5.156 267.60 0.040 4.462
Data for the solubility of mixtures of calcium sulfate and sodium chloride at
o°-09° are given by Arth and Cretien (1906).
Data for the equilibrium CaSO4 + Na2CQ3 ^ CaCO3 + Na2S04 at 25° are
given by Herz (191 la).
219 CALCIUM SULFATB
SOLUBILITY OF MIXTURES OF CALCIUM SULFATE AND SILVER SULFATE IN
WATER.
(Euler, 1904.)
Per Liter of Solution. Total Salt c r t
i°. r Cou Cms. Equiv. per 100 Gms.
Cms. Salt. Sal£ Solution Solutions.
'7°igfs°d4 -35
1:5
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND OF SODIUM SULFATE AT 25°.
(Seidell, Smith, Cameron, Brea/eale.)
In Sodium Nitrate. In Sodium Sulfate.
Gms. per Liter Solution. \yt. of T cc. Gms. per Liter Solution. \yt. of r cc.
'NaNO?. CaSO4. ' Solution. ' Na2SO4. CaS67 Solution.
o 2.08 0.9981 2.39 1.65 1.0013
25 4.25 1.0163 9-54 i-45 1.0076
50 5.50 1.0340 14.13 1.39 1.0115
100 7.10 1.0684 24.37 I-47 1.0205
200 8.79 1.1336 46.15 1.65 1.0391
300 9.28 1.1916 115.08 2.10 1.0965
600 7.89 1.3639 146.61 2.23 1.1427
655 7.24 L3904 257.10 2.65 I.2I2O
Data for the solubility of calcium sulfate, sodium sulfate glauberite, sodium
sulfate syngenite, separately and mixed, in water at various temperatures, are
given by D'Ans (1909) and;'Barre (1911).
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS AND ALCOHOLIC MONO-
POTASSIUM TARTRATE SOLUTIONS AT 20°.
(Magnanini, 1901.)
Gms. CaSO4 Gms. CaSO<
•Solvent. per 100 Gms. Solvent. per 100 Gms.
Solution. Solution.
Water 0.2238 10% alcoholic N/ 200 KHC^Oe 0.0866
Aq. N/2oo KHC^Oe 0.2323 Aq. N/2oo KHC2H4O6+s% tar-
10% alcohol 0.0970 taric acid 0.2566
10% ale. N/4oo KHC2H406+5%
tartaric acid 0.1086
SOLUBILITY OF CALCIUM SULFATE IN AQUEOUS SUGAR SOLUTIONS.
(Stolle, 1900.)
Per cent Concen- Gms. CaSC>4 Dissolved by 1000 Gms. of the Sugar Solutions at:
Solutions. 30°.
40°. 50°.
60°.
70°.
80°.
0
2.157
•73°
1.730
1.652
1.710
10
2.041
1.730
•730
i-574
i-574
1.613
20
i. 808
1.652
.419
1.380
1.419
1.263
27
i-55o
1.438 M
.361
1.283
1.283
0.972
35
1.263
1.050
.088
1.108
0.914
. . .
42
1.030
0.777
0.816
0.855
0.729
49
. . .
0.564 0.739
0.564
0.603
0.486
55
0.486 0.505
0.486
0.369
0.330
ioogms.glycerolofdi5i.256dissolve5.i7gms. CaSChat i5°-i6°. (Ossendowski, 1907.)
100 gms. glycerol of d 1.114 dissolve 0.95 gm. CaSO4 at ord. temp. (Asselin, 1873.)
CALCIUM SULFATE 220
FREEZING-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES OF CALCIUM SULFATE AND OTHER SALTS:
Calcium Sulfate + Lithium Sulfate (Mailer, 1910.)
+ Potassium Sulfate (Muller, 1910; Grahmann, 1913.)
+ Rubidium Sulfate (Muller, 1910.)
+ Sodium Sulfate (Muller, 1910; Calcagni and Mancini, 1910.)
CALCIUM SULPHIDE CaS.
SOLUBILITY IN AQUEOUS SUGAR SOLUTIONS.
(Stolle.)
Per cent Concen-
trution of Sugar /•
Grams CaS Dissolved per Liter of the Sugar Solutions at:
Solutions.
30°.
40°.
50°.
60°.
70°.
80°.
PC*.'
0
i
.982
2.123
I
•235
i
•390
1.696
2
.032
2.496
10
i
.866
I.3I6
I
.441
i
•673
1.560
I
•634
1-544
20
2
.187
I .696
I
.802
i
•905
1.879
I
.892
1.930
27
2
.522
2-097
2
•059
2
.226
2.342
2
•304
2-357
35
2
.689
2.265
2
•304
2
.406
2.342
2
•857
2.947
42
2
•342
2 .136
2
.226
2
.522
2-574
2
•509
2.689
49
2
•445
2.290
2
•458
2
.638
2.728
2
.8l8
3-o63
55
2
•509
2.226
2
•340
2
.882
2.766
2
.972
3.616
CALCIUM SULFITE CaSO32H2O.
SOLUBILITY IN WATER AND IN AQUEOUS SUGAR SOLUTIONS AT 18°.
(Weisberg, 1896.)
Grams CaSOa per 100 cc. Solution.
Solvent. ' At Too After Boiling
At l8 ' Solution 2 Hours.
Water 0.0043 ....
10 Per cent Sugar o . 0083 o . 0066
30 Per cent Sugar o . 0080 o . 0069
RESULTS AT HIGHER TEMPERATURES.
(Van der Linden, 1916.)
Cms. CaS03.2H20 per 1000 gms. Sat. Solution at.
Solvent.
30°. 40°. 50°. 60°. 70°. 80°. 90°. b. pt.
Water 0.064 0.063 °-°57 0.06 1 0.045 0-031 0.027 o.on
AqSucroseofi5gms.perioo
Water+Excess CaSC>4 0.031 0.029 0.025 0.019 0.012 0.009 0.008 0.006
0.032 0.022 0.019 0.021 0.017 0.020 0.021
Aq. Sucrose, 15 gms.+i-S gms. }
Glucose per 100 cc.+Excess > 0.032 0.027 0.022 0.020 0.019 0.019 0.019 0.023
CaSO4
CALCIUM Phenanthrene SULFONATES.
SOLUBILITY IN WATER.
(Sandquist, 1912.)
r«»v. ,,r.^ Gms. Anhydrous Salt
Compound. ^ IQQ g£ ^
Calcium- 2-Phenanthrene Monosulfonate 0.024
" - 3- " " -2H20 0.083
" -io- " " .2H2O 0.30
221 CALCIUM TARTRATE
CALCIUM TARTRATE CaC4H4O6.4H2O.
SOLUBILITY IN WATER.
(Cantoni and Zachoder, 1905.)
AO Gms. CaC«H4O«.4H2O to Gms. CaC^HtOj.^jO to Gms. CaC4H4O8.4HiO
** per ioo cc. Sol. per ioo cc. Sol. per ioo cc. Sol.
o 0.0365 30 0.0631 70 0.1430
10 0.0401 40 0.0875 80 0.1798
20 0.0475 5° o.noo 85 0.2190
25 0.0525 60 0.1262
ioo gms. aq. Ca. tartrate solution contain 0.0185 gm« CaC4H4O6.4H2Oat 18°, and
0.029489 gm. at 25°.
ioo gms. 95% alcohol solution contain 0.0187 gm. CaC4H4O6.4H2O at 18°, and
0.02352 gm. at 25°. (Partheil and Hiibner, 1903.)
ioo gms. aq. Ca. tartrate solution contain 0.0364 gm. CaC4H4O6 at 20°.
ioo gms. 10% alcohol solution contain 0.0160 gm. CaC4H4O6 at 20°.
ioo gms. aqueous 5% tartaric acid solution contain 0.1632 gm. CaC4H4O6
at 2O°. (Magnanini, 1901.)
SOLUBILITY OF CALCIUM TARTRATE, CaC4H4O6.4H2O, IN AQUEOUS ACETIC
ACID SOLUTIONS AT 26°-27°.
(Herz and Muhs, 1903; see also Enell, 1899.)
Normality of Gms. CHsCOOH Residue from Normality of Gms. CHsCOOH Residue from
Acetic Acid. per ioo cc. Sol. 50.052 cc. Sol. Acetic Acid. per ioo cc. Sol. 50.052 cc. Sol.
o o 0.0217 3.80 22.80 0.2042
0.57 3.42 0.1082 5.70 34.20 0.1844
1.425 8.55 0.1635 10.09 60.54 0.1160
2.85 17.10 0.1970 16.505 93.03 0.0337
The residue was dried at 70° C.
SOLUBILITY OF CALCIUM TARTRATE IN AQUEOUS SOLUTIONS OF CALCIUM
_j CHLORIDE, TARTARIC ACID, ETC., AT 18°.
(Paul, 1915.)
(The determinations were made by weighing the tartrate remaining undissolved
and calculating the amount dissolved by difference. It was found that even a
small amount of CO2 in the water had a distinct influence on the solubility. One
liter of pure CO2 free water was found to dissolve 0.380 gm. CaC4H4O6.4H2O at
1 8° and one liter of ordinary distilled water, 0.410 gm. at the same temperature.)
Results for Aque- Results for Aqueous Results for Aque- Results for Alcoholic
ous Calcium Dipotassium Tar- ous Tartaric Tartaric Acid
Chloride Solution.
' Gms. per Liter.
trate
Gms. per
Sols.
Liter.
Acid Sols.
Gms. per Liter.
Sols.
Gms. per Liter.
CaCU.
CaQaOe. kjC4H4O6.
CaC4H4Oe. .
4H20.
n TT n CaC4H406.
L4-n.6vJ6* TT f\
4rl2U.
CzHsOH.
OHeOe.
CaC4H4O«.
0.503
0.
202
0.392
0.166
i
0
.910
50
0
0.263
1.005
o.
179
• 2
•139
0.160
2
I
.162
(4
4
I.I07
3.518
0.
166
2
•352
o.i57
4
I
•5"
(4
16
i.8S
4.523
0.
154
2
.614
0.150
6
I
.776
80
O
0.205
o.
154
4
•705
0.223
8
I
.972
tt
4
0.867
7-538
0.
171
23
•524
0.263
10
2
.205
u
16
1.506
IO.O5
0.
177
47
.048
0.305
12
2
.380
IOO
o
0.190
25.125
o.
182
14
2
.514
u
4
0.766
50.25
0.
224
16
2
.643
14
16
1.297
Data for the effect of potassium chloride and of potassium acetate upon the
solubility of calcium tartrate in aqueous 0.5 normal acetic acid solutions at 25°,
and also for the effect of potassium monochloracetate upon the solubility of the
salt in 0.5 normal chloracetic acid solutions at 25°, are given by Henderson and
Taylor (1916).
CALCIUM TARTRATE
222
SOLUBILITY OF CALCIUM TARTRATE IN AQUEOUS SOLUTIONS OF AMMONIUM,
POTASSIUM AND SODIUM CHLORIDES AT SEVERAL TEMPERATURES.
(Cantoni and Jolkowsky, 1907.)
NOTE. — (The authors refer in all cases to their determination of the amount of
decomposition of the tartrate by the aqueous chloride solutions. Constant agita-
tion and temperature were maintained.)
Cms. Chloride per
Liter Solvent.
5
10
30
IOO
2OO
Cms. Ca Tartrate Dissolved at
16° per Liter of Aq.:
ta.
16
30
55
70
85
Cms. Ca Tartrate per Liter of
7% Aqueous:
NH4C1. KC1. NaCl
0.701 0.643 0.680
0.861 0.822 0.840
I.28l I.lSo 1.305
1.897 J-753 i -860
2.305 2. 110 2.163
NH4C1. KC1. NaCl.
1.676 1.504 1.637
2.417 2.031 2.275
3.712 2.154 3.579
5.080 2.546 4.148
6.699 4.264 6.305
CALCIUM BITARTRATE CaH2(C4H4O6)2.
SOLUBILITY IN WATER AND IN AQUEOUS SOLUTIONS OP ACIDS AND
OF SALTS.
(Warington — J. Chem. Soc. 28, 946, '75.)
In Hydrochloric Acid. In other Acids and in Salt Solutions at 14°.
Acid or Salt. GmsAcidorSalt Gms.CaH2(C4H4O6)a
per loo cc. Sol. per 100 cc. Sol.
Acetic Acid
Tartaric Acid
Citric Acid
Sulphuric Acid
Hydrochloric Acid
Nitric Acid
Potassium Acetate
Potassium Citrate
Cone, of HC
Gms. per
loo Gms. Sol
1 Gms. CaH2(C4H4O6)2
per 100 Gms. Solvent.
• At 22°.
At 80°.
O
O.6OO
4-027
0.68
3-01
5-35
2.15
6.88
"•35
4.26
11.19
20.23
8.36
22.75
40.93
16.13
48.31
80.12
0.81
0.422
1.03
0.322
0.84
0.546
0.685
1.701
0.504
1.947
0.845
1.969
1-387
0.744
1-397
0.843
CALCIUM THIOSULFATE CaS2O,.6H2O.
SOLUBILITY OF CALCIUM THIOSULFATE IN AQUEOUS SOLUTIONS OF SODIUM
THIOSULFATE AT 9° AND 25° AND VICE VERSA.
(Kremann and Rodemund, 1914.)
Results at 9°.
Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol
Solid Phase. Sat. Sol.
NazSzOj.
CaSzOa. NazSzOs.
CaSzO.
0
29.4 CaS2O3.6H2O o
34-7
II .04
22.64 " 9.24
29.69
25.21
15 .84 "+Na2S2O3.5H2O 15 .67
21.41
31.01
7.70 Na2S2O3.5H2O 18.34
25.18
28.24
21 .14
30.19
20.33
31.24
18.43
35-04
ii. 61
Results at 25°.
Solid Phase.
CaS2O3.6H2O
Data are also given for the quaternary systems, CaS2O3+Na2S2O3+NaNO3
+H2O and CaS203+Ca(NO3)2+NaNO3+ H2O at 9° and 25°. A triple salt of the
composition CaNa^SzOs^NOa.iiHaO was obtained.
223
CALCIUM VALERATE
CALCIUM VALERATE Ca[CH3(CH2)3coo]2.H2o.
CALCIUM (Iso) VALERATE Ca[(CH3)2.CH.CH2.COO]2.3HaO.
SOLUBILITY OF EACH IN WATER.
(Lumsden — J. Chem. Soc. 81, 355, '02; see also Furth — Monatsh. Chem. 9, 313, '88; Sedlitzky —
Ibid, 8, 566, '87.)
Calcium Valerate.
Gms. CaCCsHoO^a
40^ per TOO Gms. t °.
Water.
Solution.
O
9.82
8.94
o
IO
9'25
8-47
10
20
8.80
8.09
20
30
8.40
7-75
30
40
8.05
7-45
40
5°
7-85
7.28
45
57
7-75
7.19
5°
60
7.78
7.22
60
70
7-80
7.24
70
80
7-95
7-36
80
90
8.20
7.58
90
100
8.78
8.07
TOO
Calcium Iso Valerate.
Gms. Ca(CsH9O2)2
per 100 Gms.
bond
Phase.
'Water.
Solution.
26.05
2O.66
(XC.H.O.VaH.O
22.70
18.50
ti
21. 80
17.90
tt
21.68
17.82
"
22.00
18.18
"
22.35
18.42
"
19-95
16.63
GKC.H.O.kH.O
18.38
I5-52
"
17.40
14.82
tt
16.88
14.44
11
16.65
14.28
"
l6-55
14.20
"
CAMPHENE Ci0H16.
Freezing-point data (solubility, see footnote, p. i) are given by Kurnakov and
Efrenov (1912) for mixtures of camphene + methylmustard oil, camphene-f-
naphthalene and camphene + phenanthene.
CAMPHOR C10H16O d and /.
APPROXIMATE SOLUBILITY OF d CAMPHOR IN SEVERAL SOLVENTS AT ORDI-
NARY TEMPERATURE. (U. S. P., Squires; Greenish and Smith, 1903.)
Parts Camphor
Solvent. per 100 Parts Solvent.
Solvent.
o . 08-0 . 14
100
Parts Camphor per
100 Parts Solvent
Water
90% Alcohol
95% Alcohol
Ether
125
173
Carbon Disulfide Readily Soluble
Chloroform
Olive Oil
Turpentine
Glacial Acetic Acid
Lanolin
300-400
25-33
66
200
12-5 (Klose,ioo7).
Saturated solutions of d camphor and of / camphor in turpentine of ap =4.38
(in a 10 cm. tube at 18°) were found to have di& = 0.9028 and 0.9030 respectively;
the <XD in a 10 cm. tube were +23.07 and —16.52 respectively. (Jones, 1907-08.)
SOLUBILITY OF CAMPHOR IN CONCENTRATED AQUEOUS HYDROCHLORIC
ACID. (Zaharia, 1899.)
(The dissolved camphor could not be determined by evaporating and weighing the
residue on account of volatility; polarimetric methods could not be used on account
of the interference of the HC1. The author, therefore, determined the densities
(H2O at 4° in each case) of the pure solvent and saturated solution in each case,
and assumed that the difference represented the weight of camphor dissolved.
The saturated solutions were prepared by stirring the several mixtures with a glass
stirring rod, at intervals, during 6 hours.)
Densities at o°. Densities at 10°. Densities at 20°. Densities at 40°.
Solvent. Sat. Sol. Solvent. Sat. Sol. Solvent. Sat. Sol. Solvent. Sat. Sol.
27.2 %HC1
.145 I . 143
.140 I . 138 I . 135
•133
.125
.123
30.6
.164
•159
.158
•153
•153
.148
. 142
•138
33 9
34.98
]
.181
.187
. 167
.158
•175
.181
•163
.160
.169
175
•159
.158
•'57
.163
•149
•153
35-74
.IQI
. 140
•185
.148
.179
153
.167
153
36.38
' 3
•195
.126
.189
•134
.182
.140
.170
•153
36.68
.197
.Il6
.190
.124
.184
•134
CAMPHOR
224
RECIPROCAL SOLUBILITY OF CAMPHOR AND PHENOL, DETERMINED BY THE
FREEZING-POINT METHOD.
(Wood and Scott, 1910.)
(The freezing-point was determined in most cases by measuring the rate of
cooling of the mixtures and ascertaining the point at which the rate changed. The
experiments were made with very great care.)
Cms. Cms.
t"of Camphor Solid f. f Camphor
FinT GnTMix- **-• Breezing. <££ j~.
ture. ture.
Solid - t'of
Phase. Freezing.
Cms.
Sms. Mix-
ture.
Solid
Phase.
174
5
IOO
.0 CjoHwO -13
.8
7i.48C10HM0 -22
.6
52
52
i.i
158
95
.98
-26
•4, -32
70.12
"+i.i -23
.6
44
90
"
140
92
•55
-15
•9
69.32
i.i —28
-30.5
40
35
"+C6H60H
112
88
.86
— 20
.1
67.76
-15
• 7
38
57
CsHjOH
80
82
.88
-19
•3
66.64
-3
34
So
"
50
7
79
•73
-18
• 7
62.21
+5
30.31
29
5
76
.58 " -18
. 6 m. pt.
16
.1
25
40
"
— O
i
73
.37 " -20
.1
61.51
25
20
31
»
~I3
S
72
.24 " — 20
55-8o
36
.1
6
8?
"
i
i = CicHieO.CeH
Data for the above system obtained by the method of determination of the
temperature of disappearance of the last crystal, are given by Kremann, Wischo
and Paul (1915). The results are not in good agreement with the above. These
authors also give similar determinations for the systems camphor -j-resorcinol and
camphor +/S naphthol.
Data for the systems camphor + phenol + water, camphor + n butyric acid -f-
water, camphor + succinic acid nitrile -f- water and camphor + triethylamine +
water are given by Timmermans, 1907.
Freezing-point data (solubilities, see footnote, p. i) are given for the following
mixtures of camphor and other compounds.
Camphor + Borneol
+ Hydroquinone
+ Menthol
-j- « Naphthol
+ 0 Naphthol
+ a Mononitronaphthalene
+ Naphthalene
+ /3 Naphthylamine
+ Nitric Acid
+ Phosphoric Acid
+ Pyrocatechol
+ Pyrogallol
-j- Resorcinol
+ Salol
-j- Sulfur Dioxide
-j- a Trinitrotoluene
4- p Toluidine
-f- i? other compounds
BenzolCAMPHOR Enol and keto forms.
Solubility data have been used by Dimroth and Mason (1913) for determining
the transition of the tautomeric forms into each other. Results are given for the
solubility of each form in ether, acetone, ethylacetate, ethyl alcohol and methyl
alcohol.
One liter benzene dissolves 256 gms. enol benzoylcamphor at 5°, by freezing-
point method. (Sidgwick, 1915.)
(Vanstone, 1909.)
(Efremov, 1912, 1913.)
(Pawlewski, 1913.)
(Caille, 1909.)
(Caille, 1909.)
Gourniaux, 1912.)
(Zukow and Kasatkin, 1909.)
«( <C
(Efremov, 1912, 1913.)
Gourniaux, 1912.)
(Caille, 1909; Efremov, 1912, 1913.)
(Caille, 1909.)
(Bellucci and Grassi, 1913, 1914.)
(Giua, 1916.)
(Efremov, 1915, 1916.)
225 BromoCAMPHOR
BromoCAMPHOR a Ci0Hi5OBr.
APPROXIMATE SOLUBILITY IN SEVERAL ORGANIC SOLVENTS AT ORDINARY TEMP.
(U. S. P.; Squires; Beilstein; results in alcohol by Miiller, 1893.)
<ir,l^A«t Parts Bromo Camphor Solvent Parts Br<>mo Camphor per
Solvent. per IOQ parts Solvent> I00 Parts Solv;nt. ^
Alcohol 12. i at 15° Ether 50
" 19.7 " 25° Chloroform 143
130.0 " 50° Olive Oil 12.5
" 705.0" 61° 95% Formic Acid 13.6 (Aschan, 1913.)
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of /bromo-
camphor + d chlorocamphor by Padoa (1904) ; for mixtures of d bromocamphor +
/ bromocamphor by Padoa and Rotondi (1912); for mixtures of bromocamphor -j-
stearine by Batelli and Martinetti (1885); /3 bromocamphor + salol by Caille, 1909.
CAMPHOROXIME Ci0H16 : NOH d and /.
100 gms. turpentine dissolve 8.68 gms. d oxime at 18°, dn = 0.8784, ap = 2.30
in 10 cm. tube.
100 gms. turpentine dissolve 8.69 gms. / oxime at 18°, du = 0.8782, an = 18.24
in 10 cm. tube.
aD of the turpentine = 4.38 in a 10 cm. tube at 18°.
In the case of results in / amyl bromide the d^ = 1.199 in both cases and the
OD was —3.55 (10 cm. tube) for the d oxime and + 11.48 for the / oxime. The etj>
of the amyl bromide was +4.6 in 10 cm. tube at 18°. The results show that the
solubility and rotatory power of the d and / isomerides are identical in an optically
active as well as in an inactive solvent.
Freezing-point data are given for mixtures of d and / camphoroxime by Beck
(1904) and Adriani (1900).
CAMPHORIC ACID C8H14(COOH)2.
loo gms. of water dissolve 0.8 gm. C8Hi4(COOH)2 at 25°, and 10 gms. at the b. pt.
(U.S.P.)
SOLUBILITY OF CAMPHORIC ACID IN AQUEOUS SOLUTIONS OF ALCOHOL AT 25°.
(Seidell, 1908, 1910.)
Wt. % C2H5OH <fes of Gms. C8Hi4(COOH)2 Wt. % CzIfcOH <fe of Gms. CeHu (COOH)a
in Solvent. Sat. Sol. per 100 Gms. Sat. Sol. in Solvent. Sat. Sol. per 100 Gms. Sat. Sol.
o i 0.754 6o i 45
10 i i. 60 70 i , 49
20 i 6.30 80 0.995 51.20
30 i 14 90 0.980 51.40
40 i 26 96.3 0.970 50.37
50 i 31 100 0.960 50.10
SOLUBILITY OF CAMPHORIC ACID IN SEVERAL SOLVENTS.
Gms. d& of Gms.
Solvent. t°. Sat. C8Hu(COOH)2 per Solvent. t°. Sat. C8H14(COOH)2per
Sol. 100 Gms. Solvent. Sol. too Gms. Solvent.
Amyl Alcohol(iso) 25 0.907 50(3) Carbon Bisulfide 25 1.258 0.020(3)
Butyl Alcohol(iso)22.5 ... 54.1(1) Chloroform 25 ... 0.153(3)
Ethyl Alcohol o ... 84.7(1) Cumene 25 0.890 0.197(3)
15.1 ... 112(2) Ether (abs.) 25 0.922 91.40(3)
62.5 ... 147(2) 95% Formic Acid 18.5 ... 8.68(4)
Methyl Alcohol o ... 116.3(1) Ligroin 25 0.714 0.007(3)
22.5 ... 131.1(1) Nitrobenzene 25 1.2 0.5(3)
Propyl Alcohol o ... 42.2(1) Spts. Turpentine 25 0.852 1.74(3)
22.5 ... 61 (i) Toluene 25 0.862 0.15(3)
Benzene 25 0.873 0.008(3) Xylene 25 0.859 0.23(3).
(i) Timofeiew (1914); (2) Beilstein; (3) Seidell (1910); (4) Aschan, (1913).
Data for the distribution of camphoric acid between water and ether at 25° are
given by Chandler (1908). Data for the freezing points of mixtures of d and /
camphoric acid and d and / isocamphoric acid are given by Centnerszwer (1899).
CAMPHORIC ANHYDRIDE C10HuO3 d and /.
One liter of benzene dissolves 37.5 gms. d camphoric anhydride at 5°, deter-
mined by depression of the freezing-point. (Sidgwick, 1915.)
CANTHARIDINE 226
APPROXIMATE SOLUBILITY IN SEVERAL SOLVENTS AT ROOM TEMP.
(Self and Greenish, 1907.)
Cms. Cantharidine Cms. Cantharidine
Solvent. per 100 Cms. Solvent. per 100 Gms.
Solvent. Solvent.
Aq. 25% Acetone 0.02 Aq. 10% Acetic Acid 0.14
" 50% " °-10 " 45% Formic " 0.12
" 75% " °-45 Carbon Tetrachloride 0.04
Lanolin 4.4 (Kiose, 1907.)
CAOUTCHOUC.
SOLUBILITY IN ORGANIC SOLVENTS. (Hanausek, 1887.)
Gms. Caoutchouc Dissolved per 100 Gms. Solvent.
Solvent. / *—m ; N
Ceara. Tete Noire. Sierra Leone.
Ether 2.5 3.6 4.5
Turpentine 4.5 5 4.6
Chloroform 3 3.7 3
Petroleum 1.5 4.5 4
Benzene 4.4 5 4.7
Carbon Bisulfide 0.4 o o
SOLUBILITY OF CAOUTCHOUC IN MIXTURES OF BENZENE AND ALCOHOL. (Caspari, 1915.)
(Freshly prepared solutions of deresinified caoutchouc in benzene were titrated
with alcohol to appearance of two phases. The end point is sharp to within one
drop of precipitant, especially at low cones, of caoutchouc. For purposes of
converting the weights of caoutchouc to volume, the factor 0.91 may be taken.)
Results at 20°.
Gms.
Caoutchouc.
cc. CVHe.
cc. Abs. Gms.
C2HsOH. Caoutchouc
cc. CeHe.
cc. 9i<
70 Gms. rr -„ cc.92<?
a. Caoutchouc. cc 5> CzHsOI
0.032
40
17
0.206
40
II
o,
,80
40
9.6
0.080
40
15
8
0.81
40
IO
.8
2
,OI
40
8.8
0.405
40
14,
,8
2.01
40
10
.2
O
.20
40
8.1
2.404
40
14
•5
3.22
40
9
.8
4.061
40
13
,8
Results at 40°. Results at 60°.
Gms. Caoutchouc, cc. C«H«. cc. Abs. CzHsOH. Gms. Caoutchouc, cc. CeHe. cc. Abs. CjHsOH,
0.2 40 18.8 0.2 40 N2i.6
i.o 40 18.1 i 40 23.3
2 40 17.4 2 40 24.4
SOLUBILITY OF CAOUTCHOUC IN MIXTURES OF BENZENE AND ACETONE. (Caspari, 1915.)
Results at 20°. ; Results at 40°. Results at 60°.
Gms. r- TT ~ cc. Gms. ^ TT cc. Gms. r TT cc.
Caoutchouc. <*• UH*' (CHs^CO. Caoutchouc. cc' UH(>- (CH3)2CO. Caoutchouc. cc 6H6' (CH3)2CO.
o.n 20 i$-7 o.io 20 19.6 o 10 20 23
0.80 20 15.0 0.98 20 17.6 i.oi 20 26.4
1.86 20 14-7
CARBAMIDES.
SOLUBILITY IN SEVERAL SOLVENTS. (Walker and Wood. 1898.)
as Methyl phenyl carbamide (m. pt. 82°), benzyl carbamide (m. pt. 149°).
o tolyl carbamide (m. pt. 185°) and p tolyl carbamide (m. pt. 173°).
Gms. Each Carbamide Separately per 100 cc. Sat. Solution.
Solvent. t°. / * v
as Methyl Phenyl. Benzyl. p Tolyl. o Tolyl
Water 45 74 1.71 0.307 0.251
Acetone 23 29.4 3-io 2.66 0.462
Ether 22.5 2.28 °-°53 0.062 0.0162
Benzene 44-2 12.4 0.0597 °-°43 °-OI5S
100 gms. chloroform dissolve 0.6-0.7 gm- diiododithio carbamide (CSN-jH^Iz
at temp, not stated. (Werner, 1912.)
227 CARBAZOLE
CARBAZOLE (Diphenylene imide) (C6H4)2NH.
100 grams abs. alcohol dissolve 0.92 gm. (C6H4)2NH at 14°, and 3.88 gms. at
b. pt.
loo gms. toluene dissolve 0.55 gm. (C6H4)2NH at 16.5°, and 5.46 gms. at b. pt.
Freezing-point data are given for mixtures of carbazole and phenanthene by
Garelli (1894).
CARBINOL CH3OH, see Methyl alcohol, p. 435.
Trimethyl CARBINOL (CH3)3COH, Triphenyl CARBINOL (C6H5)3COH.
Freezing-point data (solubilities, see footnote, p. i) are given for mixtures of
trimethyl carbinol and water by Paterno and Mieli (1907). Results for tri-
methyl carbinol + phenol, trimethyl carbinol + thymol and trimethyl carbinol +
bromotoluene are given j^by Paterno and Ampola (1897). Results for triphenyl
carbinol + phenol are given by Yamamoto (1908).
CARBON DIOXIDE CO2.
SOLUBILITY IN WATER.
(Bohr, 1899; Geffcken, 1904; Just, 1901.)
Solubility in Water. IlNaCl% ^NaCl^
*°* ' ~ ~^ft~ ~T^ V ft. '
o 0.335 I-7I3 ••• 1-234 0.678
5 0.277 1.424 ... 1.024 0.577
10 0.231 1.194 ••• 0.875 0.503
15 0.197 1.019 1.070 0.755 0.442
20 0.169 0.878 ... 0.664 0.393
25 — 0.145 0.759 0.826 0.583 0.352
30 0.126 0.665 ... 0.517 0.319
40 0-097 °-S3° ••• 0.414 0.263
50 0.076 0.436 ... 0.370 0.235
60 0.058 0.359 ... 0.305 0.183
q •= wt. of gas dissolved by i oo grams of solvent at a total pressure of 760 mm.
ft = the Bunsen Absorption Coefficient which signifies the volume (v) of
the gas (reduced to o° and 760 mm.) taken up by unit volume (V) of the liquid
when the pressure of the gas itself minus the vapor tension of the solvent is
760 mm. _ v
* ~ V(i + 0.00367 /) '
/ = the Ostwald Solubility Expression which represents the ratio of the
volume (v) of gas absorbed at any pressure and temperature, to the volume
(V) of the absorbing liquid, i.e. I = —- This expression differs from the
Bunsen Absorption Coefficient, ft, in that the volume (v) of the dissolved gas
is not reduced to o° and 760 mm. The solubility / is therefore the volume
of gas dissolved by unit volume of the solvent at the temperature of the
experiment. The two expressions are related thus:
0.00367 /), ft =
, A
(i + 0.00367 0
SOLUBILITY IN WATER AT PRESSURES ABOVE ONE ATMOSPHERE.
(Wroblewski — Compt. rend. 94, 1335, '82.)
pressure Coefficient of Saturation* at: .Pressure Coefficient of Saturation * at :
in Atmos- , - - — — • - - — > m Atmos- . - - - • -
Dheres. ° • I2-4 • pheres. 0°- 12.4°.
i 1-797 i. 086 20 26.65 17.11
5 8.65 5.15 25 30.55 20.31
10 16.03 9-65 3° 33-74 23.25
* Coefficient of absorption is no doubt intended.
CARBON DIOXIDE
228
SOLUBILITY OF CARBON DIOXIDE IN WATER AT HIGH PRESSURES. (Sander, 1911-12.)
NOTE. — The pressures varied from 25 to 170 kilograms per square centimeter.
The results are expressed in terms of the volume of CC>2, reduced to I kg. per sq.
centimeter, dissolved by unit volume of liquid at the temperature and pressure
of the experiment. A Caillet apparatus, provided with the well-known Caillet
tube, was used. The experiments were made with very great care. In general,
the procedure consisted in compressing CO2 above mercury in the closed milli-
meter graduated end of the Caillet tube and taking many readings on the scale
at various pressures and temperatures. The volumes thus found were compared
with similar readings made after a known amount of solvent had been introduced
above the layer of mercury, by means of a graduated pipet with turned-up end.
The differences show the volume of CO2 dissolved at given temperatures and
pressures.
Two series of determinations were made. In the case of the results marked (a)
the used volume of water was 0.210 cc. and for those marked (6) the volume was
0.102 cc. The volumes of CO2 used, varied from 60 to 76 cc.
20
35
a
60
tt
SOLUBILITY OF CARBON DIOXIDE IN WATER EXPRESSED IN TERMS OF THE FAHR-
ENHEIT SCALE OF TEMPERATURE AND POUNDS PER SQUARE INCH PRESSURE.
(Heath, 1915; Anthony, 1916, see also Riley, 1911.)
(The existing data were calculated to this form, particularly for use in the
bottling industry.)
Volumes of CCfe Gas Dissolved by One Volume of Water at:
Pressure in
Kg. per
Sq. Cm.
cc. of COa (Reduced to
i Kg. per Sq. Cm.) Dis-
solved by i cc. HzO.
r.
Pressure m
Kg. per
Sq. Cm.
, Cc. CO2 (Reduced to i Kg.
per Sq. Cm.) Dissolved
by i cc- H2O.
(a)
(ft)
(a)
(6)
25
. . .
17.77
60
90
22.74
21. l6
30
. . .
19.77
u
100
26.22
27.85
40
...
21 .52
It
110
28.92
28.79
50
. . .
28.09
tl
120
30.20
33-90
55
. . .
29-75
100
00
8.97
. . .
30
11.77
13-57
tt
70
IO.II
6.40
40
14.82
20
n
80
11.05
9-59
5o
18.96
24.64
tt
90
12.62
10.85
00
22 .90
22 .50
a
100
I3-63
12.40
70
27.18
27.62
it
no
14.88
16.31
80
. . .
32.85
tt
120
16.40
15-78
40
10.88
9.80
tt
130
17-93
16.89
50
12.24
I3-72
tt
I4O
19.56
17.71
60
14.46
15.28
tt
150
20.58
17.49
70
16.80
17.46
tt
160
22.07
80
19.74
22.67
tt
170
22.78
Inch
Pressure
32°.
36°.
40°.
44°.
48°.
55°.
60°.
65°.
70°. 75°-
80°.
85°. 90°.
is
3.46
3-iQ
2.93
2.70
2tso
2. 2O
2.02
1.86
I.7I 1.58
1.84
4-35 *-27
20
4.04
3-73
3.42
3-15
2^2
2-57
2.36
2.17
2 1.84
1.69
1.58 1.48
25
4.58
4.27
3.92
3.61
3-35
2.04
2.69
2.48
2.29 2.IO
i-93
1.80 1.70
30
5.21
4.81
4.41
4.06
3-77
3.31
3.03
2.80
2.58 2.37
2.18
2.03 1.91
35
5.80
5-35
4.91
4-52
4.19
3-69
3-37
3-11
2.86 2.63
2.42
2.26 2.13
40
6.37
5-89
5-39
4.97
4.61
4.05
3.71
342
3.15 2.89
2.67
2-49 2.34
45
6.95
6.43
5.88
5-43
5.03
4-43
4.06
3-74
3-44 3-i6
2.91
2.72 2.56
5°
7-53
6-95
6.36
5-89
5-45
4.80
4.40
4.05
3-73 3-42
7.16
2.94 2.77
55
8.ii
748
6.86
6-34
5.87
5.17
4-74
4.37
4.02 3.69
3-4°
3.17 2.99
60
8.71
8.02
7-35
6.79
6. 20
>53
5.08
4.68
4-31 3-95
3-64
3-39 3-20
70
9.86
9.09
8.33
7.70
7-13
6.27
5-76
5-30
4.89 4.49
4.14
3-86 3-63
80
1 1. 02
10.17
9.3i
8.6 1
7.98
7
6-43
5.92
5.46 5.02
4.62
4.31 4.06
00
12. 18
11.25
10.30
9-52
8.82
7.74
7.11
6-54
6.04 5.55
5.12
4-77 4-49
100
13-34
12.33
11.29
10.43
9.66
8-4
7.79
7.18
6.62 6.08
<.6o
5.22 4-91
SOLUBILITY OF CO2 IN
229 CARBON DIOXIDE
AQUEOUS SOLUTIONS OF ACIDS AND SALTS.
(Geffcken.)
Aq.
Gms. Acid C02 Dissolved, / at:
Aq.
Gms. Salt
CO2 Dissolved, / at:
Solvent.
per Liter.
15°-
25°-
Solvent
per Liter.
15°.
25°.
HC1
18.23 I
.043
0.806
CsCl
84.17
I .OO6
0
.781
"
36.46 I
.028
0.799
KC1
37-30
0.976
0
•759
tt
72.92 I
.000
0-795
]£C1
74.60
0.897
o
.700
HN03
3I-52 I
.078
0.840
KI
83.06
0.992
0
•775
"
63-05 I
.086
0-853
KI
166.12
0.923
o
.727
Cl
126.10 I
.100
0.877
KBr
59-55
0.986
o
.768
H2SO4
24.52 I
.018
0.794
KBr
119.11
0.914
0
•713
tt
49 . 04 o
.978
0.770
KNO3
50.59
1.005
o
.784
t(
.98.08 o
.917
0.730
KN03
101.19
0.946
o
•749
n
147.11 o
.870
0.698
RbCl
60.47
0.989
0
.769
n
196.15 o
.828
0.667
RbCl
120.95
0.921
o
.788
SOLUBILITY IN
AQUEOUS SOLUTIONS OF SALTS. (Mackenzie, 1877.)
Salt in
Gms. Salt per
Density of
Absorption Coefficient a at:
Solution.
100 Gms. Solution. Solution 15". ' go
15°.
22°.
KC1
6.05
i .021
0.988
o-777
o
.670
tt
8.646
1-053
0.918
0.777
o
.649
"
11.974
1.080
0.864
0.720
o
•597
tt
22.506
1-549
0.688
o-57i
o
.480
NaCl
7.062
1.038
0.899
(6.4°)
o-735
it
12.995
1.080
0.633
(6.4°)
o.557
o
.482
11
17.42
1.123
0.518
(6.4°)
0.431
0
•389
tt
26.00
I-I95
o-347
(6.4°)
0.297
o
•263
NH4C1
6.465
i .021
1.023
0.825
o
.718
"
8.723
1.047
1. 000
0.791
0
.702
"
12.727
1-053
0.922
0.798
o
.684
tt
24.233
i .072
0.813
(10°)
0.738
0
.600
8°.
16-5°.
22°.
30°.
BaCl2
7.316
.068
0.969
0.744
0.680
0
.566
tt
9-753
.092
I .O2I
0.645
0.607
0
•543
tt
14.030
•137
. . .
0.618
0.524
o
.467
tt
25-215
•273
0-495
0.618
0.383
0
•315
SrCl2
9.511
.087
0-779
0.663
0
-508
tt
12.325
•1159
0-737
0.586
0.507
o
•539
n
17.713
•173
0.606
o-473
0.444
0
•367
"
3i-i94
•343
0.285
0.245
0.247
o
.223
CaCl2
4-365
.036
0.942
0-759
0.673
0
•596
tt
5-739
I
.049
0-855
0.726
0.616
0
•527
tt
8.045
I
.068
0.838
0.674
0.581
0
.500
tt
15-793
I
•*39
0.632
0.520
0.471
0
.400
Data for the solubility of CO2 in sea water are given by Hamberg (1885).
According to Fox (19093.), analyses of sea water all show an excess of base over acid, that is, when COi
Is left out of account. This COz (about 50 cc. per liter) is, of course, in equilibrium with the excess of base,
which is actually equal to about 40 rngs. OH per liter. The partial pressure of COz very seldom, if ever,
exceeds 6 in 10,000. For the determination of the absorption coefficient of COz there are, consequently,
four independent variables to be considered; influence of alkalinity, a chemical influence in addition to the
purely physical influences of temperature, pressure and salinity. For convenience, the dissolved COz may
be considered as made up of two parts, about i % dependent upon physical influences alone and a far larger
part dependent upon the alkalinity, pressure and temperature, but independent of salinity. Extensive
experimental determinations are described.
A critical review of the literature on the solubility of carbon dioxide in water
and in sea water is given by Coste (1917).
CARBON DIOXIDE
230
SOLUBILITY OF CARBON DIOXIDE IN AQUEOUS SOLUTIONS OF SALTS
(Setschenow, 1892.)
(Results expressed in terms of cc. CO2 (at o° and 760 mm.) dissolved
sat. solution.)
Salt.
Cms.
Salt per
Dis-
solved
Salt.
Cms.
Salt per
Dis-
solved
Salt.
Cms.
Salt per
Dis-
solved
Liter.
C02.
Liter.
C02.
Liter.
C02.
NH4C1
I
1.005
LCI
16.72
1-035
NaCl
12.9
0.978
M
IO
0.985
i
50.15
0.808
«
64
0.760
tt
51.6
0.941
t
125.4
0.596
t
128
0.580
tt
172
0.819
i
250.8
0.497
t
192
0.466
tt
258
0.770
i
501.5
O. I2O
NaBr
II5.I
0-775
NI^NOa
2.8
1.013
MgS04
26.5
O.9OI
1
460.3
0.364
'
II. 2
I.OO2
a
79-5
0.669
(
690.4
O.22I
<
55
0.989
it
159
0.441
NaNOa
89.3
0-835
i
IOI
0.962
n
3i8
0.188
u
J25
0.762
t
202. i
0.9II
KBr
83-9
0.908
M
208.4
0.621
i
404-3
0.807
"
167.7
0.819
U
416.8
0.385
t
810.4
0.612
u
25*. 5
0.748
ft
625.2
0.244
(NH4)2S04
72.2
0.712
tt
503.1
0-579
NaClO3
233-3
0.625
u
144.4
0.575
KI
3*9- 1
0-777
<l
349-9
0.506
Ba(N03)
62.7
0.922
tt
478.6
0.688
n
699.8
0.257
Ca(N03)2
41
0.923
tt
957-3
0.506
Na2S04
14.2
0.950
Citric Acid
12
1.007
KSCN
326
0.691
tt
94.8
0.620
49
0.975
tt
489
0.590
tt
284.4
0.234
99
0.950
it
978
0.387
ZnSO4
38.3
0.903
198
0.893
KN03
58.8
0-959
n
76.7
0.783
298
0.841
u
II7-5
0.890
tt
230
0.474
595
0.719
tt
235-1
0.781
(<
460
O.2O9
Cms. * . Solubility
Cms.
Salt per Lf ofCO2,Ost-
100 cc. g~V wald Ex-
Salt.
Salt per
too cc.
Solution, pression l^.
Solution.
0.825
Fe(S04)(NH4)2SO4.6H2O
9-51
2.35 1.005 0.791
a
10.26
5.05 1.013 0.754
it
22.47
IO.O2
.022 0.732
KC1
1.84
17.09
.045 0.665
u
3-05
2.80
.Ol8 0.789
tt
4-58
5.81
.040 O.74I
ft
7.46
8.15
.054 0.710
Sucrose
2.63
9-97
.070 0.676
tt
5.16
5-o8
.019 0.8l5
tt
9.68
10.12
.041 0.795
tt
12.33
Several determinations at other temperatures are also given.
SOLUBILITY OF CARBON DIOXIDE IN AQUEOUS SALT SOLUTIONS AT 25°.
(Findlay and Shen, 1912.)
, r Solubility
<jalf salt per ^. oiuu2, use- cn u bait per ^ f ofCO2,Ost-
oalt. ,^ ^ oat. mn-\j v^_ t>ait. 5_ bat. wai<| j?x_
„ ' pression /2B.
Water alone 0.825 Fe(SO4) (NH4)2SO4.6H2O 9.51 1.052 0.641
NH4C1 2.35 1.005 0-791 10.26 1.057 0.629
.124 0.460
.008 0.792
--.-., „ „ -017 0.764
BaCl2 2.80 .018 0.789 4.58 .026 0.749
.044 0.701
.009 0.813
.... . „ .018 0.798
Chloral Hy- ( 5.08 .019 0.815 9-68 .038 0.767
drate } 10.12 .041 0.795 I2-33 -051 0.744
Data for KC1 solutions at higher pressures are given by Findlay and Creighton,
1910.
Data for the influence of colloids and fine suspensions upon the solubility of
carbon dioxide in water at 25° and at various pressures are given by Findlay, 1908;
Findlay and Creighton, 1910, 1911; Findlay and Shen, 1911, 1912; Findlay and
Williams, 1913; Findlay and Howell, 1915.
The solubility of CO2 increases slightly with increasing concentrations of
Fe(OH)8l gelatine, silicic acid, aniline (chem. combination occurs), methyl orange,
blood, serum, peptone, protopeptone, and commercial hemoglobin. The solu-
bility diminishes slightly with increasing concentrations of arsenious sulfide,
dextrine, soluble starch, glycogen (?), egg albumen and serum albumen. No
appreciable effect is produced by suspensions of charcoal or silica.
^When the solubility is increased by a given substance, the solubility curve falls
with increase of pressure; when it is lessened, the curve rises with increasing pres-
sure. In the case of starch and other neutral colloids, the solubility passes through
a minimum with increase of pressure.
Data for the influence of colloids and suspensions on the evolution of COj from
supersaturated solutions, are given by Findlay and King, 1913-14.
231
CARBON DIOXIDE
SOLUBILITY OF CARBON DIOXIDE IN AQUEOUS SALT SOLUTIONS AT 15.5° AND
760 MM. PRESSURE.
(Christoff, 1905.)
A gravimetric method was used. A stream of CO2 was passed through the
weighed salt solution and, after saturation, the solution again weighed and the dif-
ference taken to represent absorbed CO2. The loss of water from the solution
was prevented by first passing the CC>2 through a series of U-tubes containing some
of the same solution. Constant temp, was not employed, but corrections of the
results were made for the slight variations in temp, which occurred. Absorption
flasks of special shape, graduated to hold 75 cc., were used.
Salt in Aq. Solution.
Water Alone
(NH4)2SO4
K2A12(S04)4.24H20
NH4HB2O4
CuSO4
LiCl
KBr
KC1
KI
KNO3
K2HAsO4
KH2As3O4
KH2PO4
K2HPO4
Gms. COiz
Gms. CO»
Cone, of Absorbed
Salt in Aq.
Cone, of Absorbed"
Aq. Sol. per 75 cc.
Solution.
Aq. Sol. per 75 cc.
Solvent.
Solvent.
0.1382
K.P4012
i normal 0.1237
i normal o . 1093
KHSO4
0.66
O.IO2O
i
0.0991
u
2.
O. IOOO
i
o . 1054
K2S04
0.66
0.1140
0.25
0.7672
"
i
0.1002
2
0.0751
Na4B4(>7
0.025
0.2205
I
0.1087
"
o. 125
0.5317
0-5
0.1209
"
0.25
O.85II
I
O. IO2O
M
sat. sol.
1.8285
2
O.O662
H
" -f-crysts. 3.2240
4
0.0527
NaBO2
0.25 normal 0.8122
i
0.1280
NaCl
i
o. 1050
i
O.I2I3
Na3PO4.i2H2O
i
0.5828
i
O.I2O4
Na4P2O7.ioH2O
i
o . 8463
i
O.I23I
Na4P4Oi2
i
0.0700
0.5
O. IIIO
ZnSO4
2
0.0720
i
0.0812
Sugar
O.I
o. 1225
i
0.0860
"
0-5
o. 1089
0.5 ' o.490o(?)
u
i
0.0931
SOLUBILITY OF CARBON DIOXIDE IN AQUEOUS SOLUTIONS OF SULFURIC ACID.
Results at 15.5°.
Per cent Cms. CO2
H2SO4 Absorbed per
in Solvent. 75 cc. Solvent.
2.5 0.1282
5 0.1079
10 0.0833
20 0.0755
30 0.0751
(Christoff,
Per cent
H2S04
in Solvent.
40
45
70
90
1905.)
Cms. CO2
Absorbed per
75 cc. Solvent.
0.0713
0.0725
0.0918
0-1433
Results at 20°. (Christoff, 1906.)
Per cent
H2SO4
in Solvent.
o
35.82
6l.62
95.6
96
Solubilit
Ostwald Expres-
0.9674
0.6521
0.7191
0.9924
j8 = 0.926 (Bohr, 1910.)
SOLUBILITY OF CARBON DIOXIDE IN AQUEOUS SOLUTIONS OF CHLORAL HYDRATE
AND OF GLYCEROL AT 15°.
Results in terms of the Bunsen absorption coefficient 0, and also the Ostwald
(von Hammel, 1915.)
solubility expression / (see p. 227).
In Aq. Chloral Hydrate.
In Aq. Glycerol.
CC1,.CH(OH)2 per Abs-Coef.,
100 Gms. Aq. Sol. ft5'
Solubility, (CH^CHOH per Aba. Corf.,
100 Gms. Aq. Sol.
Solubility,
17.7
0.885
0-935
0
1.008
I .064
31.6
0.803
0.848
26.11
0-785
0.829
38.3
0.781
0.825
43-72
0.639
0.675
49-8
0.760
0.802
62.14
0.511
0.540
57-i
0.765
0.808
77-75
0.430
0-454
68.8
0.797
. 0.842
90.74
0.404
0.427
79-4
0.903
0-953
99.26
0.410
0.438
CARBON DIOXIDE
232
SOLUBILITY OP CARBON DIOXIDE IN ALCOHOL.
(Bohr — Wied. Ann. Physik. [4] IP 247, 'oo)
In 99 per cent Alcohol. In 98.7 per cent Alcohol.
cc. COg (at o° and^ 760 mm.) per i cc. cc. COz (at o° and^?6o mm.) per r cc.
b .
'Alcohol.
Sat. Solution.
-65
38.41
35-93
— 2O
7-51
7.41
— 10
5-75
5-69
0
4.44
4.40
+ 10
3-57
3-55
20
2.98
2 .96
25
2.76
2-74
30
2-57
2.56
40
2.20
2.19
45
2 .01
2.00
Alcohol.
39 -89
7-25
5-43
4-35
Sat. Solution.
37-22
7.l6
5-38
4-31
SOLUBILITY IN AQUEOUS ALCOHOL AT 20°.
(Muller, 1889; Lubarsch, 1889.)
Density of Per cent Abs. Coef. Density of
Per cent Abs. Coef.
Alcohol. Alcohol by Wt. of COz, a. Alcohol.
Alcohol by Wt. of COz, a.
0.998 1.07 0.861 0.922
49.O 0.982
0.969 22.76 0.841 0.870(18.8
i°) 7I.I 1.293
0.960(22.4°) 28.46 0.792 0.835(16°)
85.3 1-974
0.956 3I-I7 0.801 0.795(19°)
99-7 2.719
o.935(i70) 42.15 0.877
SOLUBILITY IN AQUEOUS ALCOHOL
AT 25°.
(Findlay and Shen, 1911.)
Results for alcohol, Results for alcohol,
Results for alcohol,
of df| = 0.9931 of dft = 0.9929
of dft = 0.9834
(2.95 gms. per 100 cc.). (3.01 gms. per 100 cc.).
(8.83 gms. per 100 cc.).
Pr«« Solubility of COz, Prpc< Solubility of COz,
mm H OstwaldExpres- mm H Ostwald Expres-
sion /25. Sion /2o.
Pressure Solubffity of COz,
mmSHge. °StW^0dntpreS-
737 0-812 745 0.814
747 0.786
836 0.813 937 0.815
942 0.784
1073 0.811 1083 0.813
1090 0.785
1338 0.811 1357 0.812
1360 0.788
These authors also showed that the solubility of COz in wort containing 13 gms.
solids per 100 cc. is less than in water; also that the solubility of CO2 in beer is less
than in aqueous alcohol solutions of alcohol content equal to that of the beer.
SOLUBILITY OF CARBON DIOXIDE IN AQUEOUS SOLUTIONS OF NON-
ELECTROLYTES AT 20°.
Results in terms of the Bunsen Absorption Coefficient /3, see p. 227. (Usher, 1910.)
Aqueous Solu-
tion of:
Gm. ,
Mols.per d
Liter.
20 of Aq.
Absorp-
tion
Coef. 0.
Aqueous Solu-
tion of:
Liter.
20 OI AQ.
Absorp-
tion
Coef. 0.
Water Alone
0.877
Resorcinol
0-5
.0096
0.901
Sucrose
0.125
.0152
0.846
Catechol
o-S
.0107
0.868
"
o. 25
•0313
0.815
Urethan
0.5
.0037
0.869
«
0.50
•0637
0.756
Carbamide
0.5
.0072
0.864
"
I
.1281
0.649
Thiocarbamide
.0092
P-859
Dextrose
0.5
.0328
0.792
Antipyrine
0.5
• 0134
0.859
Mannitol
0.5
•0303
0.782
Acetamide
0.5
.0005
0.879
Glycine
o-S
.0141
0.843
Acetic Acid
0.5
.0026
0.868
Pyrogallol
0-5
.0172
0-853
n Propyl Alcohol
o-S c
>-9939
0.869
Quinol
0-5 ^
:.oo95
0.887
233
CARBON DIOXIDE
SOLUBILITY OF CARBON DIOXIDE IN ORGANIC SOLVENTS AT Low TEM-
PERATURES AND PRESSURES. (Stem, 1912-13.)
Very accurate determinations with an elaborate apparatus. The results are
expressed in terms of K' = the number of cc. of CO2, reduced to o°, absorbed at the
indicated pressure by I gram of liquid. This number differs from the Bunsen
absorption coefficient only by a constant factor which is the density d of the liquid.
Therefore Bunsen coef. /3 = K'd. The results are also expressed in terms of the
Ostwald solubility expression / (see p. 227).
-78
-59
SOLUBILITY OF CARBON DIOXIDE IN ORGANIC SOLVENTS AT HIGH PRESSURES.
(See Note, p. 228.) (Sander« I9"-"-)
Solvent, CjHsOH. Solvent, CHsOH.
Pressure d= 0.872. d-Jlt = 0.884-
mi£:m' <*J= 0-856. ij = 0.866.
Solvent,
(CHj)zCO.
d-ja = 0.900
d-£9 = 0.879-
Solvent,
CHsCOs.OHs.
d_p = 1.017.
<*-j9 = 0.994
Solvent.
CHjCOjCHj.
d-p= 1.056.
d-|9= 1.032.
K1.
/.
K1.
/.
K'.
/.
K'.
/.
K'.
/.
5°
107
194
120.5
3"
196.6
250.2
177-5
304.9
224.1
100
iii.S
68.4
195
119.6
322
I98.I
255-6
177.1
315
224.3
200
115-7
69.5
202.9
1 20. 1
344-5
201.5
271.8
179.2
337.4
223.1
400
123.8
71.4
221.5
122.2
400
208.8
310.9
183.2
389.3
225.6
700
138.6
74.7
260
126.8
545-5
IOO
40.85
27.27
63
42.5
97-8
67.2
85.3
65.6
94-3
75-8
2OO
41
27.16
64.2
42.7
IOI.2
68
86.3
65-3
98.45
77.1
400
42.35
27.65
66.3
43-i
106.6
72.8
91.6
66.7
103.6
77-6
700
44.15
28.10
69
43-35
II8.8
72.8
IOI.5
69.7
112.9
79
Pres-
sure in
perSq
Cm.
Cc. of COj (Reduced to i Kg per Sq. Cm.) Dissolved at the Temp, and Pressure of Experi-
ment by i cc. of Sat. Solution in:
. ClHjOH aHrOH (CjHOzO
(0.093 cc.) (0.103 cc.) (0.131 cc.)
CHsCOOCzHs QHs CeHsCl OHsBr OHsNOi
(0.155 cc.) (0.08 cc.) (0.106 cc.) (0.113 cc.) (0.164 cc.)
OHsCHa
(o.ii4cc.)
Results at 20°.
20
.
56.16
.
71.16
62.61
50.83
57-12
57-91
30
104.8
86.62
188.2
125-3
95-22
82.29
92.50
103-3
40
149.7
122. 1
227.9
192.4
137.3
121. 1
"5.9
155-9
50
188.8
174.6
264.3
187.5
1 60
155-9
235-8
Results
at 35°-
20
40
. . .
48.65
46.66
43.38
44.48
49-6
40
113.1
98.16
188.4
138.3
101.5
90-43
94-39
118.8
60
173
159-9
241.3
219.8
243-1
168.3
.146
145.1
192.1
80
269.6
233-9
227
Results
at 60°.
2O
24-73
. . .
34-57
35.86
30.58
31-38
40
72.82
64-65
140.5
88.71
73-69
62.64
52.26
78.67
60
122.5
111.5
195-4
186.7
156.6
118.1
98.73
72-15
128.1
80
167.9
159.2
221.4
223.4
215
149-3
i3J-4
85-03
171.9
IOO
195-7
213.9
248.7
284.4
169.7
210
Results at 100°.
30
33.65
30.56
41.09
28.68
40
26.5
80.70
46.52
48.16
41.49
50-36
49-25
60
66.05
74.51
IOI
132
91.27
77-24
72.64
70.85
85.98
80
III. 2
107.7
142.8
162.3
155-8
103
92.86
86.86
II7.6
IOO
145-7
144.7
175.4
i9i-5
212.9
121.5
118
. . .
149
1 20
174.6
175.4
258.2
140.7
140.7
. . .
I7I.8
130
182.6
146.8
178.2
The figures in parentheses immediately below the formulas of the solvents in the
above table, show the volumes of solvent used for the series of determinations in
each case. The volumes of CO2 varied from about 55 to 77 cc. in the several
cases. The increasing content of COa in the solvents at increasing pressures
caused a considerable increase in volume of the solvent. This was determined
and the proper calculation of the readings to the saturated solution were made.
All necessary figures to show the extent of the applicability of Henry's Law in the
present case, are given.
CARBON DIOXIDE
234
SOLUBILITY OF CARBON DIOXIDE IN ORGANIC SOLVENTS.
(Just, 1901.)
The determinations are described in great detail.
of the Ostwald solubility expression / (see p. 227).
Results are given in terms
Solvent.
fc
*».
b.
Solvent.
b.
/20-
/«.
Water
0.8256
Benzene
2.425
2.540
2.710
Glycerol
0.0302
. . .
Amylbromide
2-455
2.638
2.803
Carbon Bisulfide
0.8699 0.8888
0.9446
Nitrobenzene
2.456
2.655
2.845
lodobenzene
1.301
I-37I
1.440
Propyl Alcohol
2.498
Aniline
1.324
1-434
I-53I
Carvol
2.498
2.69O
2.914
o Toluidine
1.381
1-473
1-539
Ethyl Alcohol (97%)
2.706
2.923
3.J30
m
1.436
1.581
1.730
Benzaldehyde
2.841
3-057
3-304
Eugenol
1-539
I-653
1.762
Amylchloride
2.910
3.127
3-363
Benzene Trichloride
1.643
Isobutylchloride
3-I°5
3-388
3-659
Cumol
1.782
1.879
1.978
Chloroform
3-430
3-681
3-956
Carven
1.802
1.921
2.030
Butyric Acid
3-478
3.767
4.084
Dichlorhydrine
1.810
1.917
2.034
Ethylene Chloride
3-525
3-795
4.061
Amyl Alcohol
1.831
1.941
2.058
Pyridine
3-656
3.862
4.291
Bromobenzene
1.842
1.964
2.092
Methyl Alcohol
3-837
4-205
4.606
Isobutyl Alcohol
1.849
1.964
2.088
Amylformate
4.026
4.329
4.646
Benzylchloride
1.938
2.072
2.180
Propionic Acid
4.078
4407
4.787
Metoxylol
2.090
2.216
2.346
Amyl Acetate
4.119
4.411
4.850
E thylenebromide
2.157
2.294
2.424
Acetic Acid (glacial)
4.679
5.129
5-6i4
Chlorobenzene
2.265
2.420
2.581
Isobutyl Acetate
4.691
4.968
Carbontetrachloride
2.294
2.502
2.603
Acetic Anhydride
5-206
5.720
6.218
Propylenebromide
2.301
2.453
2.586
Acetone »>
6.295
6.921
. . .
Toluene
2-305
2.426
2-557
Methyl Acetate
6.494
SOLUBILITY OF CARBON DIOXIDE IN ETHYL ETHER, f RESULTS IN TERMS OF THE
OSTWALD SOLUBILITY EXPRESSION /.
(Christoff, 1912.)
k = 7-330.
/io = 6.044.
Data for the solubility of carbon dioxide in mixtures of acetic acid and carbon
tetrachloride and of ethylene chloride and carbon disulfide are given by Christoff,
1905.
Data for the adsorption of CO2 by p azoxyphenetol at temperatures below and
above its melting point, show that no adsorption or solution occurs while the
material is in the solid (unmelted) condition, but after the first melting, absorp-
tion takes place and as soon as the isotropic liquid phase is reached, a second very
well-marked increase in absorption is observed. After this, expansion and de-
crease of solubility proceed regularly with rise of temp. (Homfray, 1910.)
'The absorption coefficient ft of CO2 in Russian petroleum was found by
Gniewosz and Walfisz (1887) to be 1.17 at 20° and 1.31 at 10°.
Data for the absorption of CO2 by rubber and carbon are given by Reychler
(1910).
Data for the absorption of CO2 by hemoglobin are given by Jolin (1889).
Data for the distribution of CO2 between air and H2O, air and aq. H2SO4 and
air and toluene at various temperatures, are given by Hantzsch and Vagt (1901).
Data for the freezing-points of mixtures of CO2 and methyl-ether and for CO2
and methyl alcohol are given by Baume and Perrot (1911, 1914).
235
CARBON BISULFIDE
CARBON BISULFIDE CSa.
SOLUBILITY IN WATER.
(Chancel and Parmentier, 1885; Rex, 1906.)
Grams CSz per 100
cc.
[Solution.
O
5
10
IS
20
25
Cms. H2O
(Rex).
0.258
0.239
...
0.217
30
35
40
45
49
Grams CS2 per 100
cc.
Solution.
Cms. H2O
(Rex).
O.IS5
0.195
0.137
O.III
0.070
0.014
0.204
0.199
0.194
0.187
0.179
0.169
,100 cc. H2O dissolve 0.174 cc. CS>2 at 22°; Vol. of solution = 100.208, Sp. Gr. =
0.9981.
100 cc. CS2 dissolve 0.961 cc. H2O at 22°; Vol. of solution = 100.961, Sp. Gr. =
1.253. (Herz, 1898.)
SOLUBILITY OF CARBON DISULFIDE IN:
Aq. Solutions of Ethyl Alcohol at 17°.
(Tuchschmidt and Folleuins, 1871.)
Wt. per cent
Alcohol.
cc.CS,
per 100 cc.
Solvent.
Wt. per cent
Alcohol.
cc. CSj
per 100 cc.
Solvent.
t°.
100
CO
91-37
50
IO
98.5
182
84.12
30
20
98.15
132
76.02
20
25
96-95
100
48.40
2
30
93-54
70
47.90
0
35
Methyl Alcohol.
(Rothmund, 1898.)
Wt. per CS2 in:
CHiOH
CSa '
Layer.
Layer.
45.1
98.3
50.8
97.2
54-2
96.4
58.4
95-5
64
93-5
40.5 (crit. temp.) 80.5
SOLUBILITY OF CARBON BISULFIDE IN ETHYL ALCOHOL. (Guthrie, 1884.)
Gms. CSz per 100
Cms. CS2+C2H5OH.
Appearance on Cooling in Ice and
Salt Mixture.
94.94
Remains
clear
down to
-18.4
89-54
Becomes
turbid at — 14 .
4
84.89
it
" " -15-
9
79.96
(t
tt
' -16
.
i
65.11
tt
(t
" -17
.
7
59.58
Remains
clear
down to
— 20
29.92
it
ii
a ((
M
CARBON
MONOXIDE CO.
SOLUBILITY
IN WATER. (Winkler,'"i9oi.)
a <
' Absorp.
/SY'Solu-.
t .
0, "Absorp.
0', "Solu-
* • Coef." '
bility."
<7-
Coef."
bility."
9*
0
0.
03537
0.03516
o
.0044
40
0.01775
0.01647
0.
0021
5
O.
03149
0.03122
0
.0039
50
0.0l6l5
O.OI42O
O.
0018
10
0.
028l6
0.02782
0
•0035
60
0.01488
O.OII97
0.
0015
15
0.
02543
0.02501
0
.0031
70
O.OI44O
o . 00998
0.
0013
20
0.
02319
0.02266
0
.0028
80
0.01430
O.OO702
0.
0010
25
0.
02142
O.O2O76
o
.0026
90
O.OI42O
0.00438
0.
0006
30
o.
01998
O.OI9I5
o
.0024 100
O.OI4IO
O.OOOOO
O.
oooo
0 =
vol.
of CO absorbed by
I
volume of the liquid at a partial pressure
of 7&
mm. See p. 227.
ft' = vol. of CO (reduced to o° and 760 mm.) absorbed by I volume of the liquid
under a total pressure of 760 mm.
q = grams of CO dissolved by 100 grams H20 at a total pressure of 760 mm.
CARBON MONOXIDE 236
SOLUBILITY OF CARBON MONOXIDE IN WATER AND AQUEOUS SOLUTIONS.
The solubility in water, in terms of the Ostwald solubility expression (see p.
227), was found by Findlay and Creighton (1911) to be l^, = 0.0154.
Data for the solubility of CO in water at high pressures are given by Cassuto,
Data for the solubility of CO in aq. NaOH solutions are given by Fonda, 1910.
Results for the solubility of CO in aq. H2SO4 at 20° are given in terms of the
Ostwald solubility expression / by Christoff (1906) as follows:
/25 for H2O = 0.02482, /25 for 35.82% H2SO4 = 0.0114, /« for 61.62% H2SO4 =
0.00958, /25 for 95.6% H2SO4 = 0.02327 and 0.02164.
Data for the solubility of CO in ox blood and ox serum at 25° are given by
Findlay and Creighton, 1910-11.
Data for the influence of time on the absorption of CO by blood are given by
Grehaut (1894). The author passed air containing from one part CO per 1000
to one part CO per 60,000, through 100 cc. portions of blood and found that the
maximum absorption, 18.3 cc. CO per 100 cc. of blood (for the I : 1000 mixture)
occurred in three hours.
Data for the solubility of CO in aqueous hemoglobin solutions are given by
Hiifner (1895) and Hiifner and Kulz (1895).
SOLUBILITY OF CARBON MONOXIDE IN AQUEOUS ALCOHOL SOLUTIONS
AT 2O° AND 760 MM. PRESSURE.
(Lubarsch, 1889.)
Wt. % Vol. % Wt. % Vol. %
Alcohol. Absorbed CO. Alcohol. Absorbed CO.
o 2.41 28.57 1.50
9-09 1-87 33.33 1.94
16.67 1.75 50 3.20
23.08 1.68
SOLUBILITY OF CARBON MONOXIDE IN ORGANIC SOLVENTS.
Just, 1901.)
Results in terms of the Ostwald Solubility Expression, see p. 227.
Solvent.
/25.
fe
Solvent.
fe.
b.
Water
o . 02404
0.02586
Toluene
0.1808
0.1742
Aniline
0.05358
0.05055
Ethyl Alcohol
o. 1921
O.I9OI
Carbon Bisulfide
0.08314
o. 08112
Chloroform
O.I9S4
0.1897
Nitrobenzene
0.09366
0.09105
Methyl Alcohol
O.I95S
0.1830
Benzene
0.1707
o. 1645
Amyl Acetate
0.2140
0.2108
Acetic Acid
0.1714
0.1689
Acetone
0.2225
0.2128
Amyl Alcohol
0.1714
0.1706
Isobutyl Acetate
0.2365
0.2314
Xylene
0.1781
0.1744
Ethyl Acetate
0.2516
0.2419
100 volumes of petroleum absorb 12.3 vols. CO at 20°, and 13.4 vols. at 10°.
(Gniewosz and Walfisz, 1887.)
SOLUBILITY OF CARBON MONOXIDE IN ETHYL ETHER.
(Christoff, 1912.)
Results in terms of the Ostwald solubility expression, see p. 227.
/o = 0.3618. /io = 0.3842.
237
CARBON MONOXIDE
SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF ACETIC ACID AND
OTHER SOLVENTS AT 25°.
(Skirrow, 1902.)
Results in terms of the Ostwald solubility expression, see p. 227.
Mixture of Wt. % rr> Mixture of
wt. %
f*s\
Acetic Ac. CHaCOOH V~' Acetic Ac.
CHjCOOH
,co.
and: in Mixture. and:
in Mixture.
*».
Aniline 100 0.173 Chloroform
56.4
0.196
86.5 o.no
O
0.206
" 58.3 0.070 Nitrobenzene
78.4
0.156
" 17.8 0.058
49
0.130
o 0.053
0
0.093
Benzene 67.5 0.199 Toluene
74-7
0.191
33-S o.I98
56.9
0.195
19.2 0.190
20.5
0.190
o 0.174
0
0.182
V
SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF
ACETONE
AND
OTHER SOLVENTS AT 25°.
(Skirrow.)
Mixture of Acetone ^(M%£° CO. Mixture of Acetone
j in iviiXLurc. ? __ j.
By Wt. ks'
%(CH,)2CO
in Mixture.
By Wt.
CO.
In.
AniHne 100 0.238 Chloroform
66.6
0.226
79.2 0.179
26.5
0.212
44.9 o.i 10
O
O.2O7
" o 0.053 /3 Naphthol
86
0.190
Carbon Bisulfide 82 o . 236
73.1
0.169
" 50.5 0.227 Nitrobenzene
78.4
0.207
26 0.187
46.8
0-157
14.5 0.144
0
0.093
o 0.096 Phenanthrene
87.2
0.205
Naphthalene 86.7 0.199 "
75
0.183
72.6 0.187
SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF
BENZENE
AND
OTHER SOLVENTS AT 25°.
(Skirrow, 1902.)
The solubility of the CO given in terms of the Ostwald expression,
see p. 227.
Mixture of Benzene ^/^^^ CO. Mixture of Benzene
%C»H6in
Mixture.
CO.
and: ByWt." fe' and:
By Wt.
k&-
Naphthalene 100 0.174 Aniline
87-3
0.156
88.5 0.164 "
71.7
0.131
66.2 0.141
42.6
0.095
Phenanthrene 89.5 0.144 "
21.2
0.068
72.6 0.127
0
0-053
a Naphthol 96 . 5 o . 149 Nitrobenzene
71.8
0.152
87.9 0.139
0.127
j8 Naphthol 97.9 0.158
0
0.093
95 . 6 o . 149 Ethyl Alconol
47-7
0.181
0
0.192
CARBON MONOXIDE 238
SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF TOLUENE AND
OTHER SOLVENTS AT 25°.
(Skirrow, 1902.)
Mixture of Tol- CgHsCHa in Mixture. CO. Mixture of Tol- frl&CIfr in Mixture. Co.
uene and: wt. %. Mol. %. Ais- uene and: \vt. %. Mol. %. k&.
Aniline 100 100 0.182 a Naphthol 95.5 97.1 0.171
" 93-4 93- S 0.169 91.2 94.2 0.162
80. i 80.3 0.148 Nitrobenzene 81.7 85.7 0.160
55.4 55.6 0.115 So.8 58.1 0.131
25.4 25.6 0.077 2.3.7 29.3 0.108
o o 0.053 ° ° 0-093
Naphthalene 92.9 94.8 0.169 Phenanthrene 94.4 97 0.170
84.9 88.7 0.161 88.8 93.9 0.161
77.3 82.5 0.153 78.4 87.5 0.147
SOLUBILITY OF CARBON MONOXIDE IN' MIXTURES OF ORGANIC SOLVENTS AT 25°.
(Skirrow.)
% of Latter in Mixture. CO
Mixture Composed of: 'By Wt. ' By Moll £
Chloroform and Methyl Alcohol o.o 0.207
" " 13.0 0.202
100 0.196
Carbon Bisulphide and Ethyl Di Chloride 100 o . 147
75 0.157
51 0.160
18.4 0.140
'o.o 0.083
Methyl Alcohol and Glycerine o.o o.o o . 196
." 39.6 30.1 0.096
60.5 50.1 0.052
77.1 68.9 0.025
loo.o 100.0 very small
NOTE. — From the results shown in the preceding five tables, it is
concluded that the solubility of carbon monoxide in various mixtures
of organic solvents is, in general, an additive function.
CARBON OXYSULFIDE COS.
SOLUBILITY OF CARBON OXYSULFIDE IN WATER.
(Winkler, 1906.)
o 1-333 O-356 20 0.561 0.147
5 1.056 0.281 25 0.468 0.122
10 0.836 0.221 30 0.403 0.104
15 0.677 0.179
For /? and q see Carbon Dioxide, p. 227.
SOLUBILITY OF CARBON OXYSULFIDE IN SEVERAL SOLVENTS.
Solvent. t°. CC'^5ohrent Authority.
Water 13.5 80 (Hempel, 1901.)
2O 54 (Stock and Kuss 1917.)
Alcohol 22 800 " "
Toluene 22 1500 M "
HC1 Solution Of CuCl 13.5 20 (Hempel, 1901.)
i gm. KOH+2CC.H2O+2CC.C2H5OH 13 .5 7200
Pyridine ... 4.4 «
Nitrobenzene 12.0 "
239 CARBON TETRACHLORIDE
CARBON TETRACHLORIDE CC14.
SOLUBILITY IN WATER. (Rex, 1906.)
t°. o°. 10° 20° 30°
Gms. CCLj per 100 gms. H2O 0.097 0.083 0.080 0.085
RECIPROCAL SOLUBILITY OF CARBON TETRACHLORIDE, ALCOHOL AND WATER.
(Curtis and Titus, 1915.)
Alcohol was added from a weight buret to mixtures of weighed amounts of
CCU and H2O, stirred vigorously at 19.75°, until the mixture became homogeneous.
Per cent Per cent Per cent
CCU. CzHfiOH. H20.
41.94 43.19 14.89
33.07 47.68 19.25
25.46 50.50 24.04
17.00 51.95 31.05
14.02 51.56 34.42
10.53 50.97 38.50
In order to determiae the effect of temperature upon the mutual solubility, one
component was added to a known mixture of the other two, and the critical
solubility temperature determined by raising and lowering the temp, through the
critical point several times. A further amount of the third component was then
added and the critical solubility temperature again determined.
**c3B
^g = 0.5048.
"Rltin ^^ ' — _ .£ . T>~4.!~ V^v^ 4 — ^ ^
Ratio CCl4
= 1.0922.
Jxaiio „ „ ,
-JTT i.WU^.
""CsHsC
>xl
ltl° H20
Per cent
Crit.oSol."
Per cent
Crit^Sol.
Per cent
Crit. Sol.
Per cent
Crit. Sol.
H2O.
HzO.
H20.
24.25
-i'.8
12.47
2.03
6.84
12.7
47-43
44-5
24.61
+3-6
13-95
23-9
7-16
21-55
47-83
39-5
25.13
10.6
14-45
29.8
7-35
27.2
48.6
30.6
25.64
17
14.85
35-4
7-54
31-3
49.61
19.9
26.14
24-5
15-3
39-55
7.84
36.8
50.07
14.6
27.15
31-45
I5-67
42.75
8.02
39-75
50.50
9.15
28.52
35- 5(?)
16.02
45-5
8.28
44.1
51.06
1.6
The results show that temperature has very little effect on the mutual solubility
of the three components. Extensive series of determinations of refractive indices
and densities of the mixtures are also given.
Freezing-point data for CCU+C1 are given by Waentig and Mclntosh (1916).
CARMINE.
loo gms. H2O dissolve 0.13 gm. carmine at 20-25°. (Dehn, 1917.)
pyridine " 3.34 gms. " " "
50% aq. pyridine " 2.03 "
CARVACROL (CH3)2CH.C6H3(CH3)OH.
MISCIBILITY OF AQ. ALKALINE SOLUTIONS OF CARVACRQL WITH SEVERAL
ORGANIC COMPOUNDS INSOLUBLE IN WATER. (Sheuble, 1907.)
To 5 cc. portions of aq. KOH solution (250 gms. per liter) were added the given
amounts of the aq. insoluble compound from a buret and then the carvacrol, drop-
wise until solution occurred. Temperature not stated.
Composition of Homogeneous Solutions.
Aq. KOH.
Aq. Insol. Compd.
Carvacrol.
5CC.
2 cc. (= 1.64 gms.) Octyl(i) Alcohol
1.8 gms.
5"
5 cc. (= 4.1 gms.)
2.6 "
5"
2 cc. (= 1.74 gms.) Toluene
4 "
5"
3 cc. (= 2.61 gms.) "
4-8 "
5"
2 cc. (= 1.36 gms.) Heptane
4.6 «
the normal secondary octyl alcohol, i.e., the so-called capryl alcohol, CHj(CH»)t.CH(OH)CHj.
CARVOXIME
240
CARVOXIME Ci0H4:NOH d, I and i.
SOLUBILITY IN AQUEOUS ALCOHOL OF dn.6 = 0.9125 (51.6 PER CENT
C2H6OH). (Goldschmidt and Cooper. 1898.)
The determinations were made by the synthetic method. On account of the
slow rate at which melted carvoxime solidified on cooling below the melting point,
in the tubes containing the synthetic mixtures, it was possible to obtain results
which show the solubility curve for liquid carvoxime, in addition to the curves for
dextro and inactive carvoxime. The curves for these latter intersect the curve
for liquid carvoxime respectively at 51.7°, the m. pt. of dextro, and 70.5° the m.pt.
of inactive carvoxime.
Gms. Gms. Mols. Carvoxime
Carvoxime. Solvent, per 100 Gms. Solvent.
t° of Solution.
Solid Phase.
Solid.
Liquid.
0.0668 1.0868
0.0373
38.4
13-9
d Carvoxime
0.1232 1.0830
o . 0689
45-8
31-9
"
0.2026 I. 02l8
0.1202
50-3
49-8
"
0.4040 I. O2l8
0.2396
. . .
79.6
"
0.4128 0.8130
0.3077
. . .
94-5
<t
0.0657 1.0980
0.0363
54-2
i Carvoxime
O.I2I2 I.0l6l
0.0723
62.5
33-7
M
0.2715 I.OI29
0.1625
69.25
61.3
u
°-3755 1-0384
0.2192
76.6
tt
0.4496 0.7768
0.3409
...
102.9
tt
SOLUBILITY IN d LIMONENE.
(Goldschmidt and Cooper, 1898.)
Gms. Ci0H4:NOH
Gms. CioH4:NOH
t8. per 100 Gms.
Solid Phase.
t°.
per 100 Gms.
Solid Phase.
d Limonene.
d Limonene.
24.6 44.6 I
Carvoxime
48
198.7
/ Carvoxime
30 59-2 I
a
49.4
199.7
d
30.3 63.3 d
tt
55.1
325-I
I
38.4 104.3 I
u
55-9
346.6
d
39.3 103.1 d
it
58.8
560
d
43.1 130.8 /
it
63.2
1269.3
d
Freezing-point data are given for mixtures of d and / carvoxime by Adriani,
1900 and by Beck, 1904.
CASEIN.
100 gms. H2O dissolve 2.01 gms. casein at 20-25°. (Dehn, 1917.)
loo gms. pyridine dissolve 0.09 gm. casein at 20-25°. "
100 gms. aq. 50% pyridine dissolve 0.56 gm. casein at 20-25°. "
Data for the solubility of casein in aqueous NaCl solutions are given by Ryd
(1917). An abstract of experiments on the solubility of casein in dilute acids is
given by Van Slyke and Winter (1913). Results for the solubility of casein in
aqueous solutions of KOH, LiOH and Ca(OH)2 at various temperatures, are given
by Robertson, 1908.
CATECHOL oC6H4(OH)2.
Freezing-point data (solubilities, see footnote, p. i) are given for mixtures of
catechol and picric acid, catechol and a naphthylamine and catechol and p tolui-
dine by Philip and Smith, 1905.
CEPHAELINE
Salts.
SOLUBILITY IN WATER. (Carr and Pyman, 1914.)
Salt. Formula. t°.
Gms. Hydrated Salt
per zoo cc. Sat. SoL
Cephaeline Hydrochloride C28H38O4N2.2HC1.7H2O 17-18 26.5
acid C28H38O4N2.5HC1 18 about 50
Hydrobromide C28H3sO4Na.2HBr.7H2O 1 7-18 5 . 4 (dried at 100°)
24I
CERIUM ACETATE
CERIUM ACETATE, BUTYRATE, FORMATE, etc.
SOLUBILITY IN WATER.
(Wolff — Z. anorg. Chem. 45, 102, '05.)
Grams Anhydrous Salt per 100 Cms. Solution at:
Salt. Formula.
Acetate Ce(C2H3O2)3.i$H2O
Butyrate Ce(C4H7O2)3, and3H2O
Iso Butyrate Ce(C4II7O2)3.3H2O
Formate Ce(GHO2)3
Propionate Ce(C3H6O2)3.H2O, and 3H2
3-544
15°.
19.61
3.406
6.603(20.4°)
0-398(13°)
18.99
76°.
12.97
1.984
3-39
0-374(75-3°)
15-93
CERIUM AMMONIUM NITRATE (Ceri) Ce(NO3)4.2NH4NO8.
SOLUBILITY IN WATER.
(Wolff.)
Gms. per 100 Gms.
t o Solution.
Atomic Gms.Ce<NO3)4.2NH4NOa
Relation. per 100 Gms.
'
NH*.
Ce.
NH* : Ce.
Solution.
Water".
25
4
.065
15
.16
2
.08
i
58
•49
140
•9
35-2
4
•273
16
• 1C
2
.06
i
61
•79
161
-7
45-3
4
.489
16
•69
2
.08
i
64
•51
174
•9
64-5
4
-625
Us
• 4oCe
.o3CeIV
2
2
.06
•39
iCe
iCelV
66
.84
201
.6
85.6
4
•778
1*5
.i6Ce
.79CeIV
2
2
.04
•34
iCe
iCe IV
69
.40
226
.8
(22
.82 Ce
2
.08
iCe
112
6
•117
.22CeIV
2
95
iCelV
88
•03
735
•4
CERIUM AMMONIUM NITRATE (Cero) Ce(NO3)3.2N#4ttO,.4H3O.
SOLUBILITY IN WATER.
(Wolff.)
Gme. per too Gms.
t<\ Solution.
NH4.
Ce.
8-75
4.787
18.56
£•5.0
5-°9
19.80
45-o
5-53
21 -06
60-0
6.01
22-77
65.06
6. ii
23.42
AtomicRe,ation.
NIL, : C
e> ' Solution.
Water.'
1.999 :
7O.2
235-5
1-995 :
74-8
296.8
2.037 •
80.4
4IO.2
2.054 :
c 87.2
681.2
2. 022 :
89.1
817.4
CERIUM AMMONIUM SULPHATE Ce2(SO4)3.(NH4)2SO4.8H2O.
SOLUBILITY IN WATER.
(Wolff.)
Gms.
Gms.
Ce2(S04)3.(NH4)2S04
1 • per 100 Gms.
Solid
Phase.
.8H2O
M
It
22.3
35-i
45-2
Solution.
5.06
4-93
4.76
Water".
5-33
S.l8
4-99
Ce2(SO4)s .(NH4)2SO4
* • per ipo Gms.
Solid
Phase.
Solution.
Water.
45 -°
2.91
2-99
Anhydride
55-25
2 .l6
2.21
u
75-4
I .46
1.48
u
85-2
I.I7
1.18
n
CEROUS CHLORIDE
242
CEROUS CHLORIDE CeCl,.
100 cc. anhydrous hydrazine dissolve 3 gms. CeCls, with evolution of gas, at
room temp. (Welsh and Broderson, 1915.)
CERIUM CITRATE 2(CeC6H607).7H2O.
100 gms. of aq. citric acid solution containing 10 gms. citric acid per 100 cc.,
dissolve 0.3 gm. Ce(C6H6O7) at 20°. (Holmberg, 1907.)
CERIUM COBALTICYANIDE Ce2(CoC6N6)2.9H2O.
100 gms. aq. 10% HC1 (di$ '= 1.05) dissolve 1.075 Sms. of the salt at 25°.
(James and Willand, 1916.)
CERIUM FLUORIDE CeF3.
Freezing-point lowering data are given for mixtures of CeF8 + KF by Puschin
and Baskow, 1913.
CERIUM GLYCOLATE Ce(C2H3O3)3.
One liter H2O dissolves 3.563 gms. of the salt at 2O°. (Jantsch and Grunkraut, 1912-13.)
CERIUM IODATE Ce(IO3)3.
Oneliter sat. aqueous solution contains 1.456 gms.Ce(IO3)3, determined by achem-
ical method, and 1.636 gms. determined electrolytically. (Rimbach and Schubert, 1909.)
CERIUM MALONATE Ce2(C3H2O4)3 + 6H2O.
c i AO Gms. Ce2(C3H2O4)3 per
Solvent- t * ' loo Grams. Solvent.
Aq. Ammonium Malonate, containing 10 gms. per 100 cc. 20 0.2
Aq. Malonic Acid, containing 20 gms. per 100 cc. 20 0.6
(Holmberg, 1907.)
CERIUM Magnesium, etc., NITRATES.
SOLUBILITY IN CONG. AQ. HNO3 (dy = 1.325 =51. 59'Gms. HNO3 per 100 cc.) AT 16°.
(Jantsch, 1912.)
Cerium magnesium nitrate, i liter sat. solution contains 58.5 gms.[Ce(NOs)6]Mg3.24H20.
" nickel " " " 75-3 " " Ni3 "
" cobalt " " " " 103.3 " " Co, "
" zinc " " " " 111.7 " " Zn3 "
" manganese " " 178.8 " " Mn? "
CERIUM OXALATE Ce2(C2O4)3.9H2O.
One liter H2O dissolves 0.00041 gm. Ce2(C2O4)3 at 25°, determined by the elec-
trolytic method. (Rimbach and Schubert, 1909.)
SOLUBILITY OF CERIUM OXALATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AND OF OXALIC ACID AT 25°.
(Hauser and Wirth, 1908; Wirth, 1912.)
Cone of Gms. per 100 Gms.
Gms. per 100 Gms.
Aqueous Sat. Sol.
Phase Conc> of Aq> Acid'
Sat. Sol.
Solid
Phase.
Acid. CeO^ Ce2(C204)3.
'
CeO2= Ce2(C2O4)s.
O.IWH2SO4 0.0136 0.0215 Ce(C204)3.9H2Oo.m(COOH)2
0.0020 o.oo32Ce2(C2O4)3-9H2O
0-5
0.0524 0.0828
0-5
0.0083 0.0131
"
i.o
0.114 0.1802
I.O
0.0040 0.0063
"
1-445
0.1764 0.2788
3-2
(sat.)
0.0019 0.0030
"
2-39
0.3083 0.4871
0.05
+.O5«H2S(
)4o.oo3O 0.0047
"
2.9
0.4724 0.7467
* 0.05
+•5
0.0025 0.0039
it
3-9
0.6300 0.9957
0.25
+-25 "
0.0046 0.0073
"
4-32
0.7502 1. 1860
0.50 " +.05
0.0105 0.0166
"
5.3 0.9019 1.4250
0.50 " +.50
o.ooio 0.0016
"
CERIUM Dimethyl PHOSPHATE Ce2[(CH3)2PO4]6.H2O.
100 gms. H2O dissolve 79.6 gms. Ce2[(CH3)2PO4]6 at 25° and about 65 gms. at
95°» (Morgan and James, 1914.)
.243
CERIUM SELENATE
CERIUM SELENATE Ce2(SeO4)8.iiH2O.
SOLUBILITY IN WATER.
Gms.
t°. Ce2(Se04)3 per Solid Phase. t°.
loo Gms. HzO.
39-55 Ce2 (SeC^s. 1 2H2O 60
37.0 60.8
36.9
33.84
33-22
33-15
32.16
(Cingolani, 1908.) ]
Gms.
Ce2(SeO4)»
per 100 Gms.
H.O.
Solid Phase.
78.2
80.5
91
95-4
13.68 Ce2(SeO4)3.8H2O
13.12
5.53
4-56
Ce2(Se04)3.7H20
o
n. 6
12.6
26
28.8
34.2
45
45-9 31-89
CERIUM SULFATE Ce2(SO4)3.
SOLUBILITY OF THE SEVERAL HYDRATES IN WATER.
(Koppel, 1904; the previous determinations by Muthman and Rolig, 1898, and by Wyrouboff, 1901,
are shown by Koppel to be inaccurate.)
2.02
I
I
100
536
785
2.513
Gms.
Mols.
Gms.
Solution.
H20.
O
14.20
0-525
18.8
14.91
o-555
19.2
15.04
0.561
0
J7-35
0.665
15
10.61
0.376
21
8.863
0.308
31-6
6.686
0.227
45-6
4-910
0.164
5o
4-465
0.148
60
3-73
0.123
65
3-47
0.114
o
15-95
0.605
IS
9-95
o.35o
Ce2(S04)3.oH20
Solution.
mv.
20.5
8.69
0.302
40
5-6l3
0.188
60
3.88
0.129
45
8.116
0.280
60
3 .145
0.103
80
1.19
0.0382
100.5
0.46
0.0149
35
7.8
0.27
40
5 -71
0.19
50
3 .31
o.n
65
1-85
0.06
82
0.98
0.032
100.5
0.42
0.014
Solid Phase.
062(504)3^20
Ce2(S04)3.5H30
Ce2(S04)3.8H20
SOLUBILITY OF CERIUM SULFATE IN AQUEOUS SOLUTIONS OF ALKALI
SULFATES. (Barre, 1910.)
In aq. sols, of
K2SO4 at 16°.
In aq
Na2SC
isols. of
4 at 19°.
In aq. sols, of
(NH4)2SO4 at 16°.
Gms. per too Gms. H2O.
Gms. per 100 Gms. HzO.
Gms. per 100 Gms. H2O.
KzSO4.
Ce2(SO4)3.
'Na2S04.
Ce2(SO4)3.
(NH4)2SO4
. CC2(SO4)l.
0
10.747
0
9.648
0
10.747
0.178
0.956
0.328
0.637
3.464
1.026
0.510
0.432
0.684
0.259
9-323
0.782
0.726
0.250
I.09I
0.0937
19 . 240
0.748
I.29O
0.042
1.392
0.0570
29-552
0.701
0
6.949 (at 33°)
1.699
0.0303
45.6l6
0.497
2.640
0.0120
55-083
0.194
3-589
0.0065
63.920
0.090
5.660
0.0046
72.838
0.035
7.710
0.0037
The following double salts
•were found.
Ce2(S04)3,
,K2SO4.2H2O,
2Ce2(S04),.
3K2S04.8H20, Ce2(S04)3.5K2S04, Ce2(SO4)3.Na2SO4.2H2O, Ce2(SO4)3(NH4)2SO4.
8H20 and Ce2(SO4)8.5(NH4)2SO4.
CERIUM SULFATE
244
SOLUBILITY OF CERIUM SULFATE IN AQ. SOLUTIONS OF SULFURIC ACID AT 25°.
(Wirth, 1912.)
Normalit
of Aq.
IfcSO*.
v Gms. per
Sat
zoo Gms.
. Sol. Solid
TlU-««
Normality
of Aq.
HzSO4.
Gms. per 100 Gms.
Sat. Sol.
Solid
Phase.
CeCfe =
= Ce2(S04)3:
CeO2 =
Ce2(S04)3.
0.0
4
.604
7
.60 CezCSO^a-SH
zo 4
•32
2
3'
.301
Ce2(S04)3.8H2O
O.I
4
.615
7
.6l8
6
.685
0
.9115
i.
505
"
I.I
3
.64
6
"
9
.68
0
•4439
o
733
"
2.16
3
.04
5
.Ol8
15
•15
O
•145
o
239
"
CERIUM SULFONATES.
SOLUBILITY IN WATER.
Name.
(Holmberg, 1907; Katz and James, 1913.)
Formula.
Gms. Anhy-
drous Salt
per 100
Gms. H2O.
25-5
5.89
Cerium m Nitrobenzene Sulfonate Ce[C6H4(NO2)SO3]3.6H2O 15
Cerium Bromonitrobenzene Sulfonate Ce[C6H3Br(NO2)SO3i.4.2]3.8H2O 25
CERIUM TARTRATE Ce2(C4H4O6)34sH2O, also 6H2O.
SOLUBILITY IN WATER (Rimbach and Shubert, 1909, by electrolytic method)
AND IN AQ. SOLUTIONS. (Holmberg, 1907.)
Solvent.
Gms. An-
hydrous Salt
per 100 Gms.
Sat. Sol.
Solid Phase.
25
20
20
20
2O
0.005
0.7
2
0.4
O.2
Water
Aq. Am. Tartrate, 10 Gms. per 100 cc.
Aq. Am. Tartrate, 20 Gms. per 100 cc.
Aq. Tartaric Acid, 20 Gms. per 100 cc.
Aq. Tartaric Acid, 40 Gms. per 100 cc.
CERIUM TUNGSTATE Ce2(WO4)3.
Freezing-point lowering data for mixtures of Ce2(WO3)3 and PbWO4 are given
by Zambonini, 1913.
CETYL ALCOHOL Ci6H33OH.
100 gms. methyl alcohol dissolve 96.9 gms. Ci6H3OH at 23.9°. (Timofeiew, 1894.)
ethyl " 102.2 " " "
« <i ii 37
propyl " " 405 " " 39
CHLORAL HYDRATE CC13.CHO.H2O.
. SOLUBILITY IN WATER, ETHYL ALCOHOL, CHLOROFORM, AND IN TOLUENE.
(Speyers, 1902.)
Calculated from the original results, which are given in terms of gram molecules
of chloral hydrate per 100 gram mols. of solvent.
In Water.
In Alcohol.
In Chloroform.
In Toluene.
•> .
w.
s".
'w.
s. '
w.
s.
w.
s:
o
1-433
189
•7
I
.11
123.3
i
•530
3-7
0.898
3-2
5
1.460
233
.0
I
.16
130.0
i
•5*5
4.0
0.900
4-0
10
1.485
275
• o
I
•23
140.0
i
.5!0
5 .0
0.910
7.0
15
1.510
• o
I
•30
160.0
i
•505
9.0
0-915
II. 0
20
J-535
383
• 0
I
.36
185.0
i
.510
19-0
o-94
21.0
25
'•555
433
• 0
I
.42
215.0
i
. 34-o
0.97
36.0
30
1.580
480
.0
I
.49
245.0
i
•540
56.0
1.02
56.0
35
i-59
516
.0
I
•55
280.0
i
•570
80.0
I .13
80.0
40
1.605
. '
I
.60
320.0
i
•590
IIO.O
1-40
IIO-O
45
1.620
.
.
W = wt. of i cc. saturated solution, S = Gms. C2HC13.H2O per 100
grams solvent.
245 CHLORAL HYDRATE
SOLUBILITY IN SEVERAL SOLVENTS.
f0 Cms. CChCOH.HzO sl . t. Gms. tCbCOH.HjO
Solvent. t . per IOQ Gms Soivent. t . IOQ Gmg Solvent
50% Aq. Pyridine 20-25 374 (Dehn, 1917.) Ether ord. t. 200 (Squires.)
Pyridine 20-25 80.9 Oil tur- (cold 10 "
Carbon Bisulfide ord. t. i . 47 (Squires.) pentine ( hot 20
Glycerol ord. t. 200 Olive Oil ord. t. 100 "
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
chloral and water by van Rossem (1908) ; for mixtures of chloral and ethyl alcohol
by Leopold (1909); for mixtures of chloral hydrate and menthol by Pawlewski
(1893) and for mixtures of chloral hydrate and salol by Bellucci (1912, 1913).
DISTRIBUTION OF CHLORAL HYDRATE BETWEEN WATER AND ORGANIC
SOLVENTS.
Immiscible Solvents. t. Dist. Coef . c^nOrg. Solvent. Authoritv-
Water and Ether 0-30° 0.235 (Hantzsch and Vagt, 1901.)
Water and Benzene ... ... (Bubanovk, 1913.)
Water and Olive Oil ord. 4.9 (Baum, 1899.)
" " " 30° 4-3 (Meyer, 1901; 1909.)
3 16.7 (Meyer, 1901.)
" " Toluene O-200 58-74.5 (Hantzsch and Vagt, 1901.)
CHLORAL FORMAMIDE CC13.CH(OH).NH.CHO.
100 gms. H2O dissolve 5.3 gms. CC13CH(OH).NHCHO at 25°. (U. S. P.)
100 gms. 95% alcohol dissolve 77 gms.SCCl3CH(OH).NHCHO at 25°.
L.U-ttJ.1
*Ci 14*
SOLUBILITY IN
(Winkler, 1912; Roozeboom
WATER.
, 1884, 1885, 1888.)
t°.
0'.
9.
f .
Gms. Cl per
100 Gms. HjjO.
Solid Phase.
0
4.6lO
I .46
— 0.24
0.492
Ice + C1.8 aq.
3
3-947
1-25
o
0.507-0.560
C1.8 aq.
6
3.411
1. 08
2
3.644
"
9
3-031
0.96
4
0.732
a
9.6
2.980
0.94
6
0.823
u
12
2.778
0.88
8
0.917
(C
10
3-095
0.980
9
0.965-0.908
tc
15
2-635
0-835
20
1.85
u
20
2.260
0.716
28.7
3-69
" + 2 layers
25
1.985
0.630
30
1.769
0.562
40
1.414
0.451
50
1.204
0.386
60
i. 006
0.324
70
0.848
0.274
80
0.672
0.219
90
0.380
0.125
[OO
c
0
ft' = vol. of Cl .(reduced to o° and 760 mm.) absorbed by i vol. H2O at total pres-
sure of 760 mm.
q = Gms. Cl per 100 gms. H2O at a total pressure of 760 mm.
The coefficient of solubility of chlorine at 15°, determined by an aspiration
method, is given as 51.7 for carbon tetrachloride, 39.6 for acetic anhydride, 36.7
for 99.84% acetic acid, 25.3 for 90 vol. % acetic acid, 16.43 for 75 vol. % acetic
acid and 13.43 for 65 vol. % acetic acid. (Jones, 1911.)
CHLORINE 246
SOLUBILITY IN WATER.
(Goodwin, 1882.)
• ,. •
The saturated aqueous solution of the chlorine was cooled until chlorine hydrate
separated; the temperature was then gradually raised and portions withdrawn for
analysis at intervals. The chlorine was determined by iodometric titration and
the results calculated to volume of chlorine dissolved by unit volume of solvent
at the given temperature and 760 mm, pressure. Slightly different results were
obtained for solutions in contact with much, little, or no chlorine hydrate. The
following results are taken from an average curve: ,
to Solubility fo Solubility ,0 Solubility
Coefficient. . Coefficient. Coefficient.
2.5 1.76 ii 3 25 2.06
5 2 12.5 2.75 30 1.8
7-5 2.25 15 2.6 40 1.35
IO 2.7 20 2.3 50 I
SOLUBILITY OF CHLORINE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID AND OF POTASSIUM CHLORIDE.
(Goodwin.)
Coefficient (^Solubility in: ^ Results at 21°. (Mellor, 1901.)
*°- HC1. HC1 HC1 KC1 Cms. HClper Solubility of Cl.
(i.o46Sp.Gr.). (i.oSSp. Gr.). (1.125 Sp.Gr.). (20 g. per xoocc.) 1000 cc. (Ostwald/, seep. 227.)
o 4.1 6.4 7.3 1.5 o. 2.2799
5 5-i S-2 6-7 2 3.134 1.6698
10 4.1 4.5 6.1 2.2 9.402 I-50I3
15 3.5 3.9 5.5 1.6 12.540 1.5292
20 3 3.4 4-7 I-2 31-340 1-8033
25 2.5 3 4 i 125.360 2.4473
30 2 2.4 ... -0.9 219.380 3-I3*2
40 1.25 1.6 ... ... 3I3-4oi 3.8224
Goodwin also gives results for solutions of NaCl, CaCl2, MgCl2, SrCl2, Fe2Cl2,
CoCl2, NiCl2, MnCl2, CdCl2, LiCl, and in mixtures of some of these, but the con-
centrations of the salt solutions are not stated.
SOLUBILITY OF CHLORINE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE.
(Kumpf, 1882; Kohn and O'Brien, 1898.)
Coefficient of Solubility in:
9-97% NaCl. 16.01 % NaCl. 19.66% NaCl. 26.39% NaCl.
o 2.3 1.9 1.7 0.5
5 2 1.6 1.4 0.44
10 1.7 1.3 1.15 0.4
15 1.4 i. 06 0.95 0.36
20 1.2 0.9 0.8 0.34
25 0.94 0.75 0.65 0.3
50 ... ... ... 0.2
80 ... ... ... 0.05
100 cc. of 6.2 per cent CaCl2 solution dissolve 0.245 Sm- Cl at 12°.
100 cc. of 6.2 per cent MgCl2 solution dissolve 0.233 gm. Cl at 12°.
loo cc. of 6.2 per cent MnCl2 solution dissolve 0.200 gm. Cl at 12°.
For coefficient of solubility see p. 227.
247 CHLORINE
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures containing chlorine.
Chlorine + Chloroform (Waentig and Mclntosh, 1916.)
+ Ethyl Alcohol " "
-j- Methyl Alcohol "
-j- Ethyl Acetate (Waentig and Mclntosh, 1916; Maass and Mclntosh, 1912.)
+ Methyl Acetate (Waentig and Mclntosh, 1916.)
+ Ether
-j- Hydrochloric Acid (Maass and Mclntosh, 1912.)
-j- Iodine (Stortenbecker, 1888, 1889.)
+ Sulfur (Ruff and Fischer, 1903.)
-j- Sulfur Dioxide (Smits and Mooy, 1910; Van der Goot, 1913.)
-j- Sulfuryl Chloride (SO2C12) (Van der Goot, 1913.)
+ Sulfur Dioxide
-j- Stannic Chloride (Waentig and Mclntosh, 1916.)
-j- Toluene (Waentig and Mclntosh, 1916; Maass and Mclntosh, 1912.)
-j- Nitrosyl Chloride (NOC1) (Boubnoff and Guye, 1911.)
DISTRIBUTION OF CHLORINE BETWEEN CC14 AND GASEOUS PHASE AND
BETWEEN CC14 AND WATER.
(Jakowkin, 1899.)
Results for CC14 +
Gaseous Phase.
MillimolsCl per Liter.
Results for dist. between CC14 and H2O.
ist Series. 2nd Series.
Millimols per Liter. Millimols per Liter.
H2OI,ayer.
ecu.
Layer.
803.3
464.6
222.5
52.93
HzO Layer.
ecu.
Layer.
864.2
335-1
311-3
202.7
Gaseous
Phase.
O.IIOQ
O.2666
O-SS^S
0.8800
ecu
Phase.
8.908
22.46
44.14
75 -°9
Total
Cl.
58.21
38.36
23.08
10.10
• Unhydro-
lized Cl.
39-67
22.97
II .12
2.707
Total
Cl.
61.73
42.62
28.98
21.70
Unhy-
drolized Cl.
42.55
26.36
15.24
9-94
Data for the effect of HC1 upon the distribution between H2O and CC14 are
also given.
CHLORINE DIOXIDE C1O2.8H2O ± iH2O.
SOLUBILITY IN WATER.
(Bray, 1905-06.)
*° SrlS? Solid Phase. t°. ^ClO, Solid Phase.
— 0.79 Eutec. 26.98 ClO2.8H2O+Ice 15.3 87.04 ClOj.SHjOiiHjO
0 27.59 ClO2.8H2O±iH2O I0.7tr.pt. 107.9 " + liquid CIO,
1 29.48 " 14 more than > 107.9 liquid CIO,
5-7 42.10 " 10.7 116.7
10 60.05 " I more than > 108.6 "
The exact composition of the hydrate could not be determined on account of
manipulative difficulties.
Data for the distribution of C1O2 between H2O and CCU at o° and 25° are given,
also some results showing the effect of H2SO4, KC1OS and of KC1 on this distribu-
tion.
CHLORINE MONOXIDE C12O.
100 volumes of water at o° absorb 200 volumes of C12O gas.
CHLORINE TRIOXIDE C12O3.
SOLUBILITY IN WATER AT APPROX. 760 MM. PRESSURE.
(Brandan, 1869.)
t°. 8.5°. 14°. 21°. 93°.
Cms. C^Oa per ioo gms. H2O 4.765 5.012 5-445 5.651
Garzarolli and Thurnbalk, 1881, say that C12O5 does not exist, and above
figures are for mixtures of C12O and Cl.
CHLOROFORM 248
CHLOROFORM CHC13.
SOLUBILITY IN WATER.
(Chancel and Parmentier, 1885; Rex, 1906.)
AO Cms. CHCls per Density of f0 Gms. CHCls per
Liter of Solution. Solutions. • 100 Cms. HjO (Rex).
O 9.87 1.00378
3.2 8.90 ... O 1.062
17.4 7.12 1.00284 .10 0-895
29.4 7-O5 1.00280 20 0.822
41.6 7.12 1.00284 30 0.776
54-9 7-75 1.00309
S'IQO cc. H2O dissolve 0.42 cc. CHC13 at 22°; Vol. of sol. = 100.39 cc., Sp. Gr. =
1.0002.
100 cc. CHC13 dissolve 0.152 cc. H2O at 22°; Vol. of sol. = 99.62 cc., Sp. Gr. =
1.4831. (Herz, 1898.)
SOLUBILITY OF CHLOROFORM IN AQUEOUS ETHYL ALCOHOL, METHYL
ALCOHOL, AND ACETONE MIXTURES AT 20°.
(Bancroft, 1895.)
In Ethyl Alcohol. In Methyl Alcohol. In Acetone.
Per 5 cc. CzHsOH. Per 5 cc. CHsOH. Per 5 cc. (CH3)2CO
cc. H2O. cc. CHCls. cc. HjO. cc. CHCls. cc. H2O.. cc. CHCb.
10 0.20 10 o.io 5 0.16
8 0.3 5 0.48 4 0.22
6 0.515 4 0.8 3 0.33
4 1-13 24 2 0.58
2 2.51 1.49 7 i 0.955
i 4.60 1.35 8 0.79 i. 12
0.91 5 i. 12 10 0.505 i. 60
0.76 6 0.30 2.50
0.55 8 0.21 3.50
0.425 10 0.19 4
0.20 20 0.16 5
O.I25 3O.24 O.I2 IO
Data for the system chloroform, ethyl ether and water are given by Juttner,
1901.
Experiments by Schachner (1910) show that various fats (olive oil, sheep suet,
goose fat) in an atmosphere containing 0.55% CHCla vapor, dissolve 0.96-0.98
per cent CHC13 at 38.5°.
Data for the properties of solutions of CHC13 in water, saline solution, serum,
hemoglobin, etc.,|in their relation to anesthesia are given by Moore and Roaf,
(1904) and Waller (1904-05).
Freezing-point lowering data (solubility, see footnote, p. i) are given for the
following mixtures of chloroform and other compounds.
Mixture. Authority.
Chloroform + Hydrobromic Acid (Maassand Mclntosh, 1912.)
+ Hydrochloric Acid (Baume and Borowski, 1914.)
+ Methyl Alcohol
4- Methyl Ether (Baume, 1914, 1909.)
p nitrophenyl chloroform + m nitrophenyl chloroform (Holleman, 1914.)
CHOLESTEROL CwHaOH.HzO.
100 gms. H2O dissolve 0.26 gm. cholesterol at 20-25°. (Dehn.igr;.)
pyridine " 68.10 gms.
50% aq. pyridine i.io "
loo cc. HzO dissolve 0.0006 gm. cholesterol-digitonide at b. pt. (Mueller, 1917.)
100 cc. ether dissolve 0.0007 gm. cholesterol-digitonide at room temp. "
Freezing-point lowering data (solubility, see footnote, p. i) are given for mix-
tures of cholesterol acetate and phytosterol a and /3 by Jaeger, 1907. Data for
mixtures of cholesterol and oleic acid, cholesterol and palmitic acid and cholesterol
and stearic acid are given by Partington, 1911.
249
CHOLESTEROL
SOLUBILITY OF STEARIC ACID ESTER OF CHOLESTEROL IN OILS AT 37° AND
VICE VERSA. (Filehne, 1907.)
The determinations were made by adding small weighed amounts of the ester
to the oil at 60° and cooling to 36-37° while stirring continually. The additions
of the ester were repeated until a clouding just appeared at 36-37°. In the case of
the solubility of the oils in cholesterol, the composition of the sat. solution was
estimated by means of the specific gravity and the melting point.
Solvent.
t° of
Clouding.
ms. Ester
Gms. Oil or Acid per 100
0 , Gms. Sat. Solution in
per loo
Solute. Ester,
Bet. by:
'Sp. Gr.
M. pt.
3-35
Olive Oil 25.5
33-8
0.26
Oleic Acid 37
40
4.11
Castor Oil 5
1.85
o-33
Ricinic Acid 20
16
0.85
Pseudo Ricinic Acid 10
12
0.87
Crotonic Acid (5)
5
Olive Oil 37.6
Castor Oil 37.6
Oleic Acid 37.5
Ricinic (Oil) Acid 37
Pseudo Ricinic Acid 36 . 2
Crotonic (Oil) Acid 36 . 5
CHOLINE PERCHLORATE and its Nitric Ether.
100 gms. H2O dissolve about 290 gms. (CH3)3N(ClO4)CH2CH2.OHat i5°.)(Hofmann
100 gms. H2O dissolve o.62'gm. (CH3)3N(C1O4)CH2.CH2.ONO2 at 15°. \ HJjJld
100 gms. H2O dissolve 0.82 gm. at 20°. J 1911.)'
CHROMIUM ALUMS.
SOLUBILITY OF CHROMIUM ALUMS IN WATER AT 25°. (Locke, 1901.)
Per loo cc. Water.
Formula.
Grams Grams Gram
Anhydrous. Hydrated. Mols.
Potassium Chromium Alum K^C^SO^^H^O 12.51 24.39 0.0441
Tellurium Chromium Alum Te2Cr2 (804)4. 24H2O 10.41 16.38 0.0212
CHROMIUM CHLORIDES CrCl3.6H2O.
SOLUBILITY OF THE GREEN AND THE VIOLET MODIFICATIONS IN WATER AT 25°.
(Olie Jr., 1906.)
The solubility of hydrated chromium chloride depends upon the inner com-
position of the solution, that is, the relative amounts of the green and the violet
modification of the salt present in the saturated solution. These are determined
by precipitating with silver nitrate. A freshly prepared solution of the green
chloride yields only one-third of its chlorine in the cold, hence the composition of
this modification, according to Werner, is represented by the formula' [Cr(H2O)4Cl2]
C1.2H2O. The violet chloride is considered to have the composition, [Cr(H2O)e]Cl3.
A determination of the amount of each present involves precipitating one portion of
the solution at o° with silver nitrate and another portion (for total Cl) at the boiling
point. Experiments were first made with aqueous solutions of different percentage
composition of the two modifications. These were agitated at 25° and analyzed at
intervals until equilibrium was reached. The time for equilibrium varied from 18
to 40 days according to the concentrations present. The effect of temperature
and of the presence of HC1 on the transition of the green chloride was also studied.
The equilibrium in saturated solutions at 25° was determined by rubbing the
hydrated chromium chloride with a little water previously cooled to o° to a thin
mush. This was then agitated at 25° and portions removed at successive inter-
vals of time and analyzed. The results show the total chloride and per cent
present as the green modification.
25 Gms. Green Salt
+ 10 Gms. H2O.
Time of Gms. CrCls Per cent
\gita- per 100 Gms. of Green
25 Gms. Violet Salt 25 Gms. Violet Salt + locc.
+ 10 Gms. H2O. of 35% Sol. of the Green Salt.
Time of Gms. CrCla Per cent
Agita- per 100 Gms. of Green
Sat. Sol.
61.99
63.88
70.68
72.11
70.62
In a later paper Olie Jr. (1907) gives additional results at 29°, 32° and 35°.
loocc.anhydr. hydrazine dissolve I3gms. CrCU at room temp. (Welsh&Broderson.'is.)
tion. Sat. Sol.
Ihr. 58.36
4hrs. 63.27
i day 68 . 50
3 days 68 . 95
19 days 68 . 58
Salt. tion.
91-7 fchr.
75.2 i day
62.36 4 days
57-22 7 "
57-38 26 «
Salt.
i-53
8.46
30.89
37.28
Si-54
tion.
ifchr.
2 days
5 "
8 "
12 "
Sat. Sol.
65.49
70.47
76.38
73.26
71.14
Salt.
15-95
26.81
39-34
34-20
58-60
CHROMIUM TRIOXIDE 250
CHROMIUM TRIOXIDE CrO3.
SOLUBILITY IN WATER.
(Buchner, and Prins, 1912-13; Kremann, Daimer and Bennesch, 1911; Koppel and Blumenthal, 1907;
and Mylius and Funk, 1900.)
,., Gms. CrO3 c Ud I Gms. CrO3 s M
OilQ 4.0 -v«- ,-.- f^mf OOllCl AO r^^w -r^^ C*mo oOUQ
- O.Q 3.6 Ice - 43-5 49-1 Ice 50 64.55 CrO,
— 1.9 7-8 " - 60 53.3 65 64.83
— 3.7 ii. s " -155 60.5 " +CrO, 82 66
— 4.8 14.1 " — 20 61.7 CrO, 90 68.5 "
— 10.95 24.9 " o 62.24 " 100 67.4 "
— 11.7 25.2 " + 18 62.45 " 115 68.4
-18.75 33-5 " 24.8 62.88 « 122 70.7
— 25.25 39.2 " 40 63.50 193-196 IOO [decomposition
Density of solution sat. at 18° = 1.705.
100 cc. anhydrous hydrazine dissolve I gm. CrO8 with evolution of gas and
production of a black precipitate at room temp. (Welsh and Broderson, 1915.)
CHROMIUM DOUBLE SALTS.
SOLUBILITY IN WATER.
Qorgensen, 1879, 1884, 1890; Struve, 1899.)
Gms. per
Name of Salt. Formula. t°. 100 Gms.
H20.
Chlorotetraamine Chromium Chlo-
ride CrCl(NH3)4(OH2)Cl2 15 6.3
Chloropurpureo Chromium Chloride CrCl(NH3)5Cl2 16 0.65
Luteo Chromium Nitrate Cr(NH3)6(NO3)3 ? 2.6
Chloropurpureo Chromium Nitrate CrCl(NH3)5(NO3)2 17.5 1.4
Chromic Potassium Molybdate 3K2O.Cr203.i2Mo03.2oH2O 17 2.5
CHROMIUM SULFATES (ous and ic).
SOLUBILITY IN WATER.
Salt. Gms. pg^oo Gms. Solid Phase. Authority.
Chromous i2.35(ato0) CrSO4.7H20 (Moissan, 1882.)
Chromic 120 (at?0) Cr2(S04)3.i8H20 (Etard, 1877.)
CHROMIUM THIOCYANATE Cr(CNS)8.
Data for the distribution of Cr(CNS)3 between water and ether at o°-3O° are
given by Hantzsch and Vagt, 1901.
CHRYSAROBIN CjoHzeOy.
SOLUBILITY IN SEVERAL SOLVENTS.
(U. S. P.)
c , Gms. per 100 Gms. Solvent at: Gms. per too Gms.
' as». 8o°. SolVent> Solvent at 25°.
Water 0.021 0.046 Chloroform 5.55
Alcohol 0.324 0.363 (60°) Ether 0.873
Benzene 4 ... Amyl Alcohol 3.33
Carbon Bisulfide o . 43
CHRYSENE Ci8Hi2.
SOLUBILITY IN TOLUENE AND IN ABS. ALCOHOL.
(v. Becchi.)
loo gms. toluene dissolve 0.24 gm. Ci8Hi2 at 18°, and 5.39 gms. at 100°.
100 gms. abs. alcohol dissolve 0.097 Sm* CisHi2 at 16°, and 0.170 gm. at boiling
point.
251
CINEOLE
CINEOLE (Eucalyptole) Ci0Hi8O.
Freezing-point lowering data (solubility, see footnote, p. i) for mixtures of
cineole and each of the following compounds are given by Bellucci and Grassi,
(1913); phenol, a. and ft naphthol, o, m and p crespl, o, m and p nitrophenol,
o, m amidophenol, pyrocatechol, resorcinol, hydroquinone, guaiacol, o, m and p
oxybenzoic acid, methyl salicylate, phenyl salicylate, naphthalene and thymol.
CINCHONA ALKALOIDS.
SOLUBILITY OF CINCHONINE, CINCHONIDINE, QUININE, AND QUINIDINE IN
SEVERAL SOLVENTS. (Muller, 1903; see also Prunier, 1879.)
Grams of the Alkaloid per 100 Grams Solution.
Solvent. Quinine
Cinchonine Cinchonidine CjoHwNjO,. Quinidine
f~> TT -»T /-\ f* TI XT C\ A /"« IT KT f\
-19
23 a •
19 n
Hydrate.
Anhydride.
Ether
0
.10
0.211
I.6l9
0.876 0.776
Ether sat. with Hp
o
.123
0-523
5.6l8
2.794 1.629
HjO sat. with Ether
0
.025
0.0306
0.0667
0.0847 0.031
Benzene
o
•0545
0.099
0.2054
1.700 2.451
Chloroform
o
.6979
9.301
100 +
100+ 100 +
Acetic Ether
0
.0719
0.3003
4.65
2.469 1.761
Petroleum Ether
0
•0335
0.0475
0.0103
O.O2II O.O24I
Carbon Tetra Chloride o
.0361
0-0508
0.203
0.529 0.565
Water
o
.0239
0.0255
o-574
0.0506 O-O2O2
Glycerine (15^°)
o
•50
0.50
... ...
SOLUBILITY OF CINCHONINE AND
CINCHONIDINE' IN SEVERAL SOLVENTS.
Gms. Alkaloid per 100
Solvent.
t°.
Gms
. Solvent.
Authority.
Cinchonine. Cinchonidine.
Water
ord. temp
. 0.0043
(Hatcher, 1902.)
u
20
0.0131
(Scholtz, 1912.)
"
25
O.OII3
0.021
(Schaefer, 1910.)
Aq. 10% Ammonia
20
0.025
...
(Scholtz, 1912.)
Aq. 85% C2H50H+io% Am.
20
0.41
...
«
Aniline
20
1.6
«
Pyridine
20
1.4
7*78
(Scholtz, 1912; Dehn, 1917.)
50% Aq. Pyridine
20-25
10
(Dehn, 1917.)
Aq. 85% C2H5OH (^20=0.832)
20
0.86
. . .
(Scholtz, 1912.)
C2H5OH (95%)
2O
0.80
5
(Wherry and Yanovsky.igiS.)
C2H5OH (prob. 92.3 wt. %)
25
0.62
(Schaefer, 1913.)
Abs. QjHsOH
19
0.874
(Timofeiew, 1894.)
Abs. C2H5OH
25
0.89
(Sill, 1905.)
Benzene
25
0.057
0.127
(Schaefer, 1913.)
Acetone
25
0.091
(Sill, 1905.)
Chloroform
17
0.014
(Oudemans, 1872.)
"
25
0.606
19
(Schaefer, 1913.)
u
SO
0-565
(Kohler, 1879.)
Ether
25
0-055
(Sill, 1905.)
"
32
0.264
(Kohler, 1879.) »
Isoamyl Alcohol '
25
I.IO
(Sill, 1905.)
Isobutyl Alcohol
1.09
.
(Timofeiew, 1894.)
Methyl Alcohol
Piperidine
25
20
0.785-1.
3-5
17 7-39
(Schaefer, 1913; Sill, 1905.)
(Scholtz, 1912.)
Diethyl Amine
2O
"
Results for the solubility of cinchonine and Cinchonidine in mixtures of ethyl and
methyl alcohols with benzene and with chloroform are given by Schaefer (1913).
It is pointed out by Schaefer (1910), that if the saturated solution is analyzed
by shaking out with chloroform or ether, variable results, depending on the age
and method of manufacture of the alkaloid, will be obtained.
Except in the case of the results by Sill in the above table, the saturated solu-
tions were obtained by agitating at intervals, instead of constantly at the given
temperature.
CINCHONA ALKALOIDS
252
SOLUBILITY OF CINCHONINE, CINCHONIDINE AND CINCHOTINE SALTS IN WATER.
Cms. per 100 Cms. H2O.
Salt.
Hydrobromide
*"• Cinchonine Cinchoni- Cinchotine Authority.
Salt. dine Salt. Salt.
25 1.7 I • 66 ... (Schaefer, 1910.)
Bihydrobromide
25
55-5 14-3
Hydrochloride
25
4 . S1 4 . 82 2 . 1 23 (Schaefer, 1910; Forst and Bohringer, 1881.)
Bihy drochloride
25
62.5 ... (Schaefer, 1910.)
Sulfate
25
I . IT4 I .o85 3 . 286 (Schaefer, 1910; Forst and Bohringer, 1881.)
Sulfate
80
3.1 4.8 ... (U.S. P.)
Bisulfate
2S
66.6 IOO ... (Schaefer, 1910.)
Perchlorate
12
0.3(solvent =aq.6% HCIOJ (Hofmann, Roth, Hobold and Metzler, 1910.)
Salicylate
25
0.17 0.075 ••• (Schaefer, 1910.)
Tannate
2S
0.091 0.055
Tartrate
25
3 . 127 ... 1 . 768 (Schaefer, 1910; Forst and Bohringer, 1881.)
Bitartrate
16
0.99 ... 1.28 (Forst and Bohringer, 1 88 1.)
Oxalate
20
0.96 ... 1.16 " "
i 4.16 at 10°. * 4 at 15°,
, » at 10°. * 1.52 at 13°. • i at 15°. • at 13°. T 3 at 16°. « at 16°.
SOLUBILITY OF CINCHONINE SULFATE AND OF CINCHONIDINE SULFATE IN
ALCOHOL AND OTHER SOLVENTS.
Gms. per 100 Gms. Solvent.
Solvent. t°.
Ethyl Alcohol (92.3 wt. %)
« « «
Methyl Alcohol
Chloroform
Ether
Glycerol
25
60
25
25
25
15
(CJBaNjO)r
H2S04.3H,0.
0.85 (1.4)
... (3-1)
35-9
O.I (O.ll)
O.O2
Authority.
(Schaefer, 1913; U. S. P.)
(U. S. P.)
(Schaefer, 1913; U. S. P.)
(Schaefer, 1913; U. S. P.)
(U. S. P.)
4.2
9.8 (10)
... (19.2)
83.9
0.66(1.45)
0.04
6.7
Results for mixtures of alcohol, chloroform and benzene are given by Schaefer, '13.
Very carefully determined data for the solubility of Cinchonine in ethyl alco-
hol, methyl alcohol, amyl alcohol and acetone solutions of various concentra-
tions of a large number of organic acids and of phenols are given by Sill, 1905.
CINNAMIC ACID C6H6CH:CH.COOH.
loo gms. H2O dissolve 0.0495 gm. C6H6CH:CHCOOH at 25°. (De Jong, 1909.)
loo gms. H2O dissolve 0.0607 gm. C«HiCH:CHCOOH at 25°. (Sidgwkk, 1910.)
loo cc. 0.5 n sodium cinnamate solution dissolve 0.155 gm. C6H5CH:CHCOOH
at 25° (Sidgwick, 1910.)
loo cc. sat. sol. in petroleum ether (b. pt. 3O°-7o°) contain 0.095 Sm- C6H6CH:
CH.COOH at 26°.
100 cc. sat. sol. in carbon tetrachloride contain 2.172 gms. C6H6CH:CH.COOH
at 26°. (De Jong, 1909.)
loo cc. sat. sol. in 95% formic acid contain 3.76 gms. C6H6CH :CH.COOH at 20°.
(Aschan, 1913.)
SOLUBILITY OF CINNAMIC ACID (Melting point, 133°) IN ALCOHOLS. (Timofeiew, 1894.)
Gms. Cinnamic Acid per 100 Gms. Sat. Solution in:
-18
-12.5
o
+ 19-5
SOLUBILITY OF CINNAMIC ACID IN ORGANIC SOLVENTS AT 25°. (Herz and Rathmann, 1913.)
So.ven,
CH3OH.
C^OH.
C3H7OH. (CH^CH.CHjOH.
8.1
6.74
4-3
. . .
9-3
8
5-5
. . .
13
n-3
8.2
. . .
22.5
18.1
13-4
8.6
loo cc. Sat. Sol. CHC13
Chloroform 1 2 . 09
Carbontetrachloride i . 75
Trichlorethylene 6 . 04
Tetrachlorethylene 2.55
Tetrachlorethane 11.05
Pentachlorethane 5 . 54
IOO C
C.+ 0 CC
80
+ 20
50
+ So
33-3
+ 66.6
20
+ 80
0
-f-ioo
n^VTVil
>cc.Sat.
Ft FrrF
Sol. l^nC
\» C2HC15
12.09
IOO C
C.+ 0 CC.
9.86
80
+ 20 "
6.61
So
+ 50 "
4-50
33-3
+ 66.6"
3.32
20
+ 80 "
1-75
o
+ IOO
per i oo cc.
Sat. Sol.
6.04
5-91
5-85
5-82
5-70
5-54
253 CINNAMIC ACID
OINNAMIO ACID C6H5CH:CH.COOH.
SOLUBILITY OF CINNAMIC ACID IN AQUEOUS SOLUTIONS OF SODIUM
ACETATE, BUTYRATE, FORMATE, AND SALICYLATE AT 26.4°.
(Philip — J Chem. Soc. 87, 992, '05.)
Calculated from the original results, which are given in terms of
molecular quantities per liter.
Gms. NaSalt
Urns. (J
per Liter in bolutio
us of:
per Liter.
CH3COONa.
C3H7COONa.
HCOONa.
Ce^.OH.COONa,
O
0.56
0.56
0.56
0.56
I
1.50
1-30
0.92
0.62
2
2.12
1.85
1. 12
0.70
3
2.52
2.25
1.27
o-73
4
2-85
2.60
1.40
0.77
5
3-05
2.90
1.47
0.80
5 ... ... ... 0.90
i liter of aqueous solution contains 0.491 gm. C6H6CH :CH.COOH
at 25° (Paul).
SOLUBILITY OF 'CINNAMIC ACID IN AQUEOUS SOLUTIONS OF ANILIN
AND OF PARA TOLUIDIN AT 25°.
(Lowenherz — Z. physik. Chem. 25, 394, '98.)
Original results in terms of molecular quantities per liter.
In Aqueous Anilin. In Aqueous p Toluidin.
Grams per Liter. Grams per Liter.
CeHfiCH : CHCOOH. CeH^CHsNIfc. QHeCH : CHCOOH.
0 0.49 o 0.49
1 1.20 I 1.52
2 1.65 2 2. 2O
3 2.02 3 2.83
4 2.35 4 3.35
6 2.92 5 3 .80
"Freezing-point data for mixtures of cinnamic acid and dimethylpyrone and
for hydrocinnamic acid and dimethylpyrone are given by Kendall, 1914.
BromoCINNAMIC ACIDS.
SOLUBILITY OF a AND OF /3 BROMOCINNAMIC ACIDS IN WATER AT 25°.
(Paul, 1894.)
Per looo cc. Sat. Solution.
Gms. Millimols.
a C6H5CH: CBrCOOH 3.9325 17.32
/3C6H5CBr: CHCOOH 0.5255 2.315
SOLUBILITY OF a I so BROMOCINNAMIC ACID IN AQUEOUS SOLUTIONS OF
OXANILIC ACID (Melting point = 120°) AT 25°.
(Noyes, 1890.)
Normality of Solutions. Grams per Liter.
C,H5NHCO- C6H5CH- QHsNHCO- QHjCH-
COOH. CBrCOOH. COOH. CBrCOOH.
o 0.0176 o 3-995
0.0275 0.0140 4.54 3.178
0.0524 0.0129 8.65 2.928
CINNAMIC ACIDS
254
Allo CINNAMIC ACIDS (Unstable Isomers of Cinnamic Acid).
SOLUBILITY OF EACH OF THE THREE ISOMERIC ALLOCINNAMIC ACIDS AND OF
THE MELTS OF THE THREE ISOMERS IN WATER.
Results for:
(Meyer,
1911.)
Allocinnamic Acid Allocinnamic Acid
Allocinnamic Acid
Melted
Allocin-
of M. pt. 68°.
of M. pt. 58°.
of M. pt. 42°.
namic Acid.
(Natural Isocinnamic Acid.)
(Artificial Isocinnamic Acid.)
fco " Cms. Acid
AO ~ Gms. Acid
+o Gms. Acid
AO Gms. Acid
per Liter.
1 ' per Liter.
per Liter.
i .
per Liter
18 6.88
18 7.62
18 8.95
18
I3-63
25 8.45
25 9-37
25 11-03
25
14.44
35 H-I4
35 I2-39
35 14-61
35
16.05
45 14.46
45 16.09
45
i8.ii
55 18.45
55
20.55
These curves
intersect that for the melted acid at the
65
23-43
melting points of
the solid isomers.
75
27.69
The results show that the three isomers are polymorphic modifications of the
cis acid.
loo gms. ligroi'n (b. pt. 60-70°) dissolve more than 16 gms. isocinnamic acid.
(Liebermann, 1903.)
IOO gms. ligroi'n (b. pt. 60-70°) dissolve approx. 2 gms. allocinnamic acid. '
SOLUBILITY OF a CHLOROCINNAMIC ACID, ETC., IN BENZENE.
(Stoermer and Heymann, 1913.)
Gms.
Gms.
Name of Compound.
M.pt.
t°.
Cmpd. per
loo Gms.
Name of Compound.
M.pt.
tf.
Cmpd. per
loo Gms.
C6H6.
C6H6.
a
Chlor-
137
2O
2.6
ft Brom-
*35
jo
1.58
Allo a
Allo a
0
Brom-
Chlor-
cin-
namic
Acid
in
120
142
21
2O
17
II
5-17
5 6.9
1.94
Allo
cis
trans
cis
Dichlor-
u
Dibrom-
cin-
namic
Acid
159-5
121
101
IOO
14
13
14
14
0.86
6.1
21.2
26.9
Mo ft
u
132
16
3-i7
trans
"
136
14
10.6
FREEZING-POINT DATA (Solubility, see footnote, p. i) FOR MIXTURES OF CIN-
NAMIC ACID AND OTHER COMPOUNDS, AND OF CINNAMIC ACID DERIVATIVES
AND OTHER COMPOUNDS.
(Bruni and Gorni, 1899.)
(de Kock, 1904.)
a Monochlorcinnamic Aldehyde + a Monobromcinnamic Aldehyde (Kiister, 1891.)
Cinnamylidine + Diphenylbutadiene (Pascal, 1914.)'
+ Diphenyldiacetylene "
Cinnamic Acid + Phenylpropionic Acid
p Methoxycinnamic Acid + Hydroquinone
CITRIC ACID (CH2)2COH(COOH)3.H20.
SOLUBILITY OF HYDRATED AND OF ANHYDROUS CITRIC ACID, DETERMINED
SEPARATELY, IN AQUEOUS SOLUTIONS 'OF ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Results for Hydrated Citric Acid. Results for Anhydrous Citric Acid.
Wt °7 C.H OH rL nf Gms- (CHo^COH- Wf „ r „ ^u j t Gms. (CH2)2COH-
inlS™ Sal! Sol. C^^ffi^° inloS°H Sats°ol. (C°°^ll^GmS'
0
•311
67-5
20
1.297
62.3
20
.286
66
40
I .246
59
40
•257
64-3
60
I.I9O
54-8
50
•237
63-3
70
1.160
52.2
60
.216
62
80
i .120
48.5
70
.192
60.8*
90
1.065
43-7
80
.163
$8.1*
IOO
i .010
38.3
90
.125
54.7*
IOO J
.068
49-8*
* Solid phase dehydrated more or less completely.
255
CITRIC ACID
SOLUBILITY OF HYDRATED AND OF ANHYDROUS CITRIC ACID, DETERMINED
SEPARATELY, IN SEVERAL ORGANIC ACIDS AT 25°. (Seidell, 1910.)
Results for Hydrated Citric Acid. Results for Anhydrous Citric Acid.
GmscoHl2)2" Gms'
sf?°Sfol(COOH)3-H°0 Solvent. <£ §f <ggsgJH
• per loo sat. bol. periooGms<
Gms. bat. Sol. Sat. Sol.
0.8917 5.980 Amyl Acetate 0.8861 4.22
0.8774 *5-43Q Ether (abs.) 0.7160 1.05
0.9175 5.276 Chloroform 1.4880 o
0.7228 2.174 C6H6, CS2
i . 4850 o . 007 CCU or CeHsCHa ... o
Solvent.
Amyl Acetate of ^20=0.8750
Amyl Alcohol of ^20=0.8170
Ethyl Acetate of d25= 0.89 1 5
Ether (abs.) of ^22=0.7110
Chloroform of d& - 1 . 476
loo gms. 95% formic acid dissolve 12.25 gms. citric acid at 20°. (Aschan, 1913.)
I oo gms. dichlorethylene dissolve o.oosgm. citric acid at 15°. (Wester & Bruins, '14.)
trichlorethylene 0.012 ' " .
" methyl alcohol " 197 gms. " " "19°. (Timofeiew, 1914.)
propyl alcohol "62.8
DISTRIBUTION OF CITRIC ACID BETWEEN WATER AND ETHER. (Pinnow, 1915.)
Results at 15°.
Mols. Citric Acid per Liter.
.
In H2O Layer. In Ether Layer.
0.902 0.0077
0.460 0.0036
O.22O O.OOI7
0.297 0.0023
COBALT AMINES.
SOLUBILITY IN WATER AT ORDINARY TEMPERATURE.
IZ7
128
I29
129
Results at 25.5°.
Mols. Citric Acid per Liter.
Dist Coef.
114
155
155
158
In H2O Layer.
°v9l75
0.481
0.241
0.315
In Ether Layer.
0.0063
0.0031
0.00155
0.0020
(Lai De, 1917.)
Name of Isomeride.
Formula.
Triamine Cobalt Nitrate [(NH3)3Co(NO2)3]
1.2 Dinitrotetraamine cobaltitetranitrodi- ["„ (NO^al'^
amine cobaltiate
1.6 Dinitrotetraamine
amine cobaltiate
Hexa-amine cobaltihexanitrocobaltiate
Gms. Isom-
eride per
liter Sat. Sol.
2.882
cobaltitetranitrodi-
r
LC°
(NH,)
" " 0.398
[Co(NH3)6]m— [Co(NO2)6]I1i 0.0215
COBALT DOUBLE SALTS.
SOLUBILITY IN WATER.
(Jorgensen — J.pr.Chem. [2] 18, 205, '78; 19, 49, '79; Kurnakoff — J. russ. phys. chem. Ges. 24, 629,
'92.)
Name.
Formula.
Co(NH3)6Cl3
Chloro purpureo cobaltic bromide CoCl(NH3)5Br2
Bromo purpureo cobaltic bromide CoBr(NH3)5Br
Chloro tetra amine cobaltic chloride
Chloro purpureo cobaltic chloride CoC^NH^gCL,
Chloro purpureo cobaltic chloride CoCl(NH3)5C
Chloro purpureo cobaltic chloride
Luteo cobaltic chloride
Luteo cobaltic chloride
Roseo cobaltic chloride
Roseo cobaltic chloride
Chloro purpureo cobaltic iodide
Chloro purpureo cobaltic nitrate
Chloro purpureo cobaltic sulphate
Nitrato purpureo cobaltic nitrate
Co(NH3)5(OH2)CI3
Co(Nttl(C*gC£
CoCl(NH3)5I2
CoCl(NH3)5(NO3)2
CoCl(NH3)5SO4.2H2O
Co(NO3)(NH3)(NOa)2
14.3
16
o
15.5
46 6
o
46-6
o
16.2
19.2
15
17.3
16
Gms. Salt
per 100
Gms. H2O.
0.467
0.19
2 . 50
0.232
0.41
i .03
4-26
12 . 74
16 . 12
24.87
2.0
i . 25
o .75
o .36
COBALT ACETATE 256
COBALT ACETATE Co(CH3COO)2.
100 cc. anhydrous hydrazine dissolve I gm. cobalt acetate with evolution of
gas' at room temp.
COBALT BROMIDE CoBr2.
SOLUBILITY IN WATER.
(Etard, 1894.)
(Welsh and Broderson, 1915.)
59°.
66 7
7S°-
66.8
97°.
68.1 (blue)
Cms. CoBr2 per 100 gms. solution
100 gms. methyl acetate (di* = 0.935) dissolve 10.3 gms. CoBr2 at 18°,
sat. solution = 1.013.
COBALT CHLORATE Co(ClO3)2.
SOLUBILITY IN WATER.
(Naumann, 1909.)
Gms.
to Co(C103)2
per 100 Gms.
Mols.
Co(C103)2
per 100
(Meusser, 1902.)
Solid Phase. t°.
Solution.
Mols
. H20.
—
12
29
•97
3
.41
Ice
18
—
21
53
•30
9
.08
Co(C103)2.6H20
21
—
19
53
,61
9
.20
«
35
0
57
•45
10
•75
"
47
10-5
61
•83
12
.90
H
61
Gms.
Mols.
t°.
Co(ClO3)2
per 100 Gms.
Co(rc!S!2 Solid phase-
Solution.
Mols. H2O.
18
64.19
14.28 Co(C103)2.4HjO
21
64.39
TACT "
35
67.09
16.10
47
69.66
18.29
61
76.12
25-39
Density of solution saturated at 1 8° = 1.861.
COBALT PerCHLORATE Co(ClO4)2.9H2O.
SOLUBILITY IN WATER.
(Goldblum and Terlikowski, 1912.)
Gms. Gms.
r>.
UKL,
Gms.
roo
H20.
Solid Phase.
t°
£
.tensity (
at. Sol.
<
JU(UUJ2
per loo
5ms. H2O
Solid Phase.
— 10
•9
32
.67
Ice
0
•564
IOO
CoCClO^.sHjO
-30
-7
58
.16
"
7-5
.566
101.9
"
-62
. 2 Eutec.
Ice+Co(C104)2.9H20
18
.567
103.8
«
-30
-7
83
.2
Co(C104)2.9H20
26
•581
113-4
H
— 21
•3
QO
.6
M
45
.588
115
H
COBALT CHLORIDE
SOLUBILITY IN WATER.
(Etard — Compt. rend. 113, 699, '91; Ann. chim. phys. [7] 2, 537, '94.)
t°.
Gms.
CoCl2 per
loo Gms.
Solid
Phase.
t°.
Gms.
CoCl2 per Solid
zoo Gms. Phase.
Solution.
Solution.
— 10
27.0
CodydHjO (red)
35
38.0 CoC^.Hp (violet)
0
29-5
14
40
41.0
+ 10
31-5
««
So
47-o
20
33-5
U
60
47-5 CoCL^O (blue)
25
34-5
it
80
49-5
30
35-5
((
TOO
51.0
SOLUBILITY OF COBALT AMMONIUM CHLORIDES IN WATER.
(Kurnakoff — J. russ. phys. chem. Ges. 24, 629, '93; J. Chem. Soc. 64, ii, 509, '93.)
Grams per 100 Grams H2O at:
o°. 16.9°. 46.6°-
,, .
CoCl3.5NH3.H2O
CoCl^NH,
0.232
16.12
4.26
24.87
1.031
...
12.74
257
COBALT CHLORIDE
SOLUBILITY OF COBALT CHLORIDE IN AQUEOUS HYDROCHLORIC
ACID SOLUTIONS AT o°.
(Engel — Ann. chim. phys. [6] 7, 355, '89.)
Milligram Mols.
per 10 cc. Sol.
Sp. Gr. of
gQpnftlflBB.
Gms. per 100 Gms.
Solution.
Gms. per 100 cc.
Solution.
iCoCl2.
HCL
CoCl2.
HCl.
CoCl2.
HCl.
62.4
O
I
•343
30
•17
0
.00
40
•5
0
58-52
3
•7
I
.328
28
.62
0
.102
38
.0
0-135
50.8
ii
•45
I
•299
25
•39
0
.321
33
.0
0.417
37-25
25
.2
I
.248
19
•43
0
•738
24
.2
0.919
12.85
55
• O
I
.167
7
•JS
z
.718
8
•34
2.OO
4-75
74
•75
I
.150
2
.68
2
•369
3
.08
2.72
12.0
104
•5
I
.229
6
•34
3
.099
7
•79
3-8i
25.0
139
•o
I
•323
12
.27
3
.829
16
.24
5-07
SOLUBILITY OF COBALT CHLORIDE IN AQUEOUS ALCOHOL
AT 11.5°.
(Bodtker — Z. physik. Chem. 22, 509, '97.)
10 gms. of CoCl2.6H2O were added to 20 cc. of alcohol and in addition
the amounts of CoCl2 shown in the second column. The solutions were
shaken 2 hours, 5 cc. withdrawn, and the amount of dissolved CoCl,
determined by evaporation and weighing.
Vol. %
Gms. CoCl2
Gms. per 5 cc. Solution.
Vol.
%
Gms. CoCl2
Gms. per 5 cc. Sol.
Alcohol.
Added.
H20.
CoCl2.
Alcohol.
Added.
H20.
CoCl2.
9x-3
0
.0
I
•325
1.168
99
•3
0.612
0
.764
1-459
98-3
O
.0
I
• 134
1.214
99
•3
0.813
0
.688
1.568
98-3
O
• O
I
.068
1.181
99
•3
I .022
o
•634
i-7i3
99-3
0
.0
I
•045
1.199
99
•3
I .240
0
•553
1.831
99-3
O
.194
O
.899
1.204
99
•3
1.446
o
•483
1-943
99-3
0
.400
O
.829
1-325
99
•3
1.650
o
.500
2.183
100 gms. sat. solution in alcohol (6.792 Sp. Gr.) contain 23.66 gms.
CoCL, So. Gr. = I.OI07. (Winkler — J.pr. Chem. 91. 207, '6*0
SOLUBILITY OF COBALT CHLORIDE IN ORGANIC SOLVENTS.
Solvent.
Acetone
Ethyl Acetate
Ether, Abs.
Glycol
Acetonitrile 18
Methyl Acetate 18
95% Formic Acid 20 . 5
Anhy. Hydrazine ±15
Gms. per 100 Gms. Solvent.
'
' CoCl2.
CoCl2.2H2O.
0
9.II
I7.I6
22.5
9.28
17.06
25
8.62
18
2-75
14
0.08
. . .
79
0.26
...
0.021
0.201
10. 7 (per 100 g. sol.)
4.08
0.369* ...
6.2
I ...
dja sat. sol. = 0.938.
Authority.
(von Laszczynski, 1894.)
(von Laszczynski, 1894.)
(Krug and McElroy, 1892.)
(Naumann, 1904.)
(von Laszczynski, 1894.)
«
(Bodtker, 1897.)
(de Coninck, 1905.)
(Naumann and Schier, 1914.)
(Naumann, 1909.)
(Aschan, 1913.)
(Welsh and Broderson, 1915.)
COBALT CHLORIDE
258
SOLUBILITY OF COBALT CHLORIDE IN PYRIDINE.
(Pearce and Moore, 1913.)
r.
Gm. CoCl2
per too Gms
Sat. Sol.
Solid
Phase.
t°
p^oo^p^l t°.
Gm. CoCl2
per 100 Gms
Sat. Sol.
Solid
• Phase.
48
.2
0
C6H5N
34
6
0.749 1.4 74.8
2.
037
1.2
50
• 3
Eutec. ...
"+ 1.6
.37
6
0.754 78.2
2.
276
"
45
0.4185
1.6
44
6
0.950 ' 79.8
2.
428
H
30
0.4205
"
47
2
.O2O
88
3-
284
"
.6
0.4208
"
.no
90 tr.
Pt. ..
" +CoCl,
10
0.4310
"
55
.192
96.5
7-
251
CoCl2
0
0.4307
«
60
.324
98.8
7-
936
"
15
tr
. pt. ...
1.6+1.4
64
2
.460
106
12.
540
M
23
0.569
1.4
68
.572 no
14.
165
•
25
0-575
"
70
tr.
pt . . . " +1.2
1.6 = CoCl2.6CsHsN. 1.4 = CoCl2.4CsHiN. 1.2 =.CoCl2.2C5H5N.
COBALT CITRATES.
Salt.
Formula.
IN WATER.
(Pickering, 1915.)
Gms. per TOO cc. Sat. Sol.
t°. ~ _ Salt
Co ~ (anhydrous).
Cobalt Citrate (normal) Co3[(COO.CH2)2C(OH)COO]2.2H2O 10 0.08 0.267
Cobalt Hydrogen Citrate CoH[(COO.CH2)2C(OH)COO] 10 0.20 0.906
Cobalt Potassium Citrate KCof(COO.CH2)2C (OH) COO]. 4H2O 10 1.05 5.11
Cobalt Potassium Citrate K4Co[(COO.CH2)2C(OH)COO]2 10 3.04 31
COBALT FLUORIDE CoF2.4H2O.
100 gms. sat. solution in water contain 2.23 gms. of cobalt fluoride of a variety.
loo gms. sat. solution in water contain 2.32 gms. of cobalt fluoride of 0 variety.
(Costachescu, 1910.)
OOBALT IODATE Co(IO3)2.
SOLUBILITY IN WATER.
(Meusser — Ber. 34, 2435, '01.)
Solid Phase :
Co(IO3)2.2H2O.
Co(IO3>.4H2O.
Co(IO3)2.
G.
o-54
0.83
1.03
1.46
1.86
2.17
M.
O.O28
0.038
0-046
0.065
0.084
0-098
G.
M.
G.
M.
0.32
O.OI4
o-45
0.020
1.03
0.046
0.52
0.023
0.89
0.040
0.67
0.030
0.85
0.030
O
18
30
So
60
65
75
100
G = Gms. Co(IO3)2 per 100 gms. solution.
per 100 Mols. H2O.
OOBALT IODIDE CoI2.
SOLUBILITY IN WATER.
(Etard — Compt. rend. 113, 699, '91; Ann. chim. phys. [7] 2, 537, *g4<)
The accuracy of these results is doubtful.
0.84
1.02
0.038
0.045
o-7S
0.69
0-033
0-031
M = Mols. Co(IO8)8
Gms. CoI2
f.
per 100 Gms.
Solution.
-10
55-5
O
58.0
10
61-5
15
63.2
20
65-2
2$
67
Solid Phase.
25
30
40
50
80
no
Gms. CoI2
per 100 Gms.
Solution.
67-5
7O.O
75-o
79.0
80.0
81.0
Solid Phase.
(olive)
ii
CoI2.H20 (yellow)
259 COBALT MALATE
COBALT MALATE Co(COO.CH2.CHOHCOO).2H2O.
ioo cc. sat. solution in water contain 0.14 gm. Co = 0.453 gm- anhydrous salt
at 10°. (Pickering, 1915.)
COBALT MALONATES.
SOLUBILITY OF COBALT MALONATES IN WATER.
(Lord, 1907.)
Gms. Anhy-
Satt. FomuJa. f. ££**..
Sat. Sol.
Cobalt Malonate CoCH2(COO)2.2H2O 18 1.353
" Ammonium Malonate Co(NH4)2[CH2(COO)2]2.4H2O 18 10.61
" Caesium " CoCs2[CH2(COO)2]2.4H2O 18 14.23
" Potassium " CoK2[CH2(COO)2]2.4H2O 18 4.26
OOBALT NITRATE Co(NO3)2.
SOLUBILITY IN WATER.
(Funk — Wiss. Abh. p. t. Reichanstalt 3, 439, *oo.)
Gms. Mols. Gms. Mols.
*' • PS°Sf^.(52^> **""-• •'• P£»S. C^S *»«*-
Solution. Mols.H2O. Solution. Mols.H2O.
— 26 39-45 6.40 Co(NO3)2.QH2O 41 55.96 12.5 Co(NO3)2.6H2O
-20.5 42-77 7-35 " 56 62.88 16.7
— 21 41-55 6-98 Co(NO3)2.6HaO 55 61.74 15.8 Co(NOa)2.3HaO
— io 43.69 7.64 " 62 62.88 16.7
- 4 44.85 7.99 " 70 64.89 18.2
o 45-66 8.26 " 84 68.84 21.7
+ 18 49.73 9.71 91 77-21 33-3
Density of solution saturated at 18° = 1.575.
SOLUBILITY OF COBALT NITRATE IN GLYCOL.
(de Coninck, 1905.)
ioo grams saturated solution contain 80 gms. cobalt nitrate.
COBALT RUBIDIUM NITRITE Rb3Co(NO2)6.H2O.
ioo gms. H2O dissolve 0.005 Sm- of the salt. (Rosenbladt, 1886.)
COBALT OXALATE Co(COO)2.
ioo gms. 95% formic acid dissolve 0.04 gm. Co(COO)2 at 19.8°. (Aschan, 1913.)
COBALT SULFATE CoSO4.7H2O.
SOLUBILITY IN WATER.
(Mulder; Tobler, 1855; Koppel, Wetzel, 1905.)
Gms. CoSO4 per
t°. ioo Gms.
Mols. CoSO4.
per ioo
Gms. CoSO4 per
t°. ioo Gms.
Mols. CoSO,
per ioo
Solution.
Water.'
Mols. H2O
Solution.
Water.
Mols. H2O.
0
20-35
25-55
2.958
35
31.40
45-80
5-31
5
21.90
28.03
3-25I
40
32.81
48.85
5.664
10
23.40
30-55
3-540
50
35.56
55-2
15
24.83
33-05
3.831
60
37.65
60.4
20
26.58
36.21
4.199
70
39-66
65-7
25
28.24
39-37
4.560
80
41.18
70
...
30
29.70
42.26
4.903
IOO
45-35
83
• • •
IOO gms. H2O dissolve 37.8 gms. CoSO4 at 25°. (Wagner, '1910.)
Freezing-point data (solubility, see footnote, p. i) for mixtures of CoSC>4 +
Li2SO4, CoSO4 + K2S04 and CoSO4 + Na2SO/are given by Calcagni and Marotta
(1913).
COBALT SULFATE
260
SOLUBILITY OP MIXTURES OP CoSO4.7H2O AND Na2SO4.ioH2O
IN WATER.
(Koppel; Wetzel.)
Gms. per
^o^ ioo Gms. Solution.
Gms. per
ioo Gms. H2O.
Mols. per
ioo Mols. H2O.
Solid Phase.
'CoSO4. Na2SO4.
rCoS04.
Na2SO4.
CoSO4.
Na2SO4.
0
5
16
17
•56
.46
9-59
21.85
23-94
10
•07
2
2
•54
•77
I
I
•27
.67
CoS04.7H20 +
Na2S04.ioH2O
10
.90
n-73
25-41
16
•67
2
•94
2
.11
..
20
17
•59
16.43
26.65
24
.91
3
.09
3
.15
CoNa2(S04)2.4H20
25
17
.06
I5-70
25.36
23
•32
2
•95
2
•97
"
30
J5
•94
14-93
23 -!5
21
.61
2
•7o
a
•74
««
35
15
•73
14.52
22.54
20.85
2
.62
2
.64
"
40
14
•87
14.22
20.98
2O
•05
2
.46
2
•53
»
18-5
18
•75
15.61
28.61
23
.82
3
•32
3
.02
CoNa2(SO4)2.4H2O
20
19
•30
15.10
29.42
23
.01
3
.41
2
.92
+ CoSO4.7H2O
25
20.30
13.60
30-74
20
•58
3
•56
2
.61
30
21
.67
12.05
32.70
18
•17
3
•79
2
•30
„
35
22
.76
10.43
34.06
15
.61
3
•95
I
.98
M
40
24
•05
9.16
35-oi
13
.72
4
.81
I
•74
"
18.5
16
.87
16.97
25-50
25
•65
2
.96
3
•25
CoNa2(S04)2.4H2O
20
15
.41
18.12
23.18
27
.26
2
.69
3
•45
+Na2S04.ioH2O
25
10
•63
23.26
16.07
35
17
I
.86
4
.46
lt
30
6
.01
28.67
9.20
43
•74
I
.07
5
•54
M
35
4
•56
32.14
7.19
50
79
O
•835
6
•44
CoNa2(SO4)2.4H2O
40
4
.72
3I-78
7-45
So-
10
o
.864
6
•34
+ Na2SO4
SOLUBILITY OF COBALT SULPHATE IN METHYL AND ETHYL ALCOHOL
AND IN GLYCOL.
Solvent.
Methyl Alcohol (abs.)
3
15
18
(93-5%) 3
(50%) 3
Ethyl Alcohol (abs.) 3
Glycol
Gms. per 100 Gms.
Solvent.
Observer.
CoSO4. CoSO4.7H2O.
. . „ 42 .8 (deBruyn — Z. physik.Ch. 10, 784, '92.)
50.9
1-04 54-5
i3-3
1.8
2.5
o . (per 100 gmS. (de Coninck— Bull. acad. roy . Belgique,
solution) 3 . i 359. '05-)
COBALT SULFIDE CoS.
One liter water dissolves 0.00379 Sm- CoS at 18° (electrolytic conductivity
method, assuming complete dissociation and hydrolysis). (Weigel, 1906.)
261
COCAINE
COCAINE C17H21N06.
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent.
Water
50% Glycerol
Gms. CnH21NO,
t°. per zoo Gms. Authority.
Solvent.
2O
0.028
(Zalai, 1910.)
±20
0.140
(Baroni and Barlinetti, 1911.)
25
0.17
(U. S. P.)
80
0.38
«
±20
8
(Baroni and Barlinetti, 1911.)
25
2O
(U. S. P.)
25
26.3
"
18-22
n. 6
(Muller, 1903.)
l8-22
34
»
18-22
0.254
"
20
76
(Scholtz, 1912.)
2O
31-94
(Gori, 1913.)
18-22
100 +
(Muller, 1903.)
18-22
100
»
18-22
59
«•
18-22
2-37
"
20-25
80+
(Dehn, 1917; Scholtz, 1912.)
20
56
(Scholtz, 1912.)
20
36
"
20
4-34*
(Zalai, 1910.)
25
8-3
(U. S. P.)
25
7.1
"
* Per too cc.
3 Cms. H3BO3 in A<
Alcohol (92.5 Wt. %)
Ether
«
Ether sat. with H2O
Water sat. with Ether
Aniline
Carbon Tetrachloride
Chloroform
Benzene
Ethyl Acetate
Petroleum Ether
Pyridine
Piperidine
Diethylamine
Sesame Oil
Olive Oil
Oil of Turpentine
COCAINE HYDROCHLORIDE C17H21NO4.HC1.
100 gms. H2O dissolve 250 gms. of the salt at 25° and 1000 gms. at 80°. (U. S. P.)
100 gms. 92.3% alcohol dissolve 38 gms. salt at 25° and 71 gms. at 60°. (U. S. P.)
100 gms. chloroform dissolve 5.4 gms. salt at 25°. (U.S. P.)
100 gms. glycerol dissolve 25 gms. salt at 15°. (B. P.)
COCAINE PERCHLORATE C17H2iNO4.HClO4.
100 gms. H2O (containing 8% free HC1O4) dissolve 0.26 gm. perchlorate at 6°.
(Hofmann, Roth, Hobold and Metzler, 1910.)
CODEINE Ci8H21NO3.H2O.
CODEINE PHOSPHATE Ci8H2iNO3.H8PO4.2H2O.
CODEINE SULFATE (Ci8H2iNO3)2.H2SO4.5H2O.
SOLUBILITY OF EACH SEPARATELY IN SEVERAL SOLVENTS.
Gms. per 100 Gms. Solvent.
e.
(U. S. P.; Baroni and Barlinetto,
(Zalai. 1910.) [1911-)
(U. S. P.)
(Schaeffer, 1913; U. S. P.)
(U. S. P.)
(Schaeffer, 1913.)
Solvent.
Water
Alcohol (92.3 Wt. %)
25
20
80
25
60
25
25
20
25
25
Codeine,
o . 80-1 . 7
0.84
1.70
63.7
108.7
62.8
2.94-1.33
8
11.4
12
C. Phos-
phate.
44-9
227
0.383
1.03
O.OI5
0.075
C.
Sulfate.
3-3
16"
O.I
0.27
0.56
0.007
Insol.
Authority.
Methyl Alcohol
Chloroform
Carbon Tetrachloride
Ether
Benzene
Trichlorethylene
3 Gms. HsBOs per 100 cc.
aq- 50% Glycerol ord. t.
loo gms. trichlorethylene dissolve 0.014 £m- codeine hydrochloride at 15°.
(Wester and Bruins, 1914.)
Data for the solubility of codeine and codeine sulfate in mixtures of alcohols,
benzene and chloroform are given by Schaeffer (1913).
0.007 (Schaeffer, U. S. P.)
(Gori, 1913; Beilstein, Suppl.)
(U. S. P.)
(Schaeffer, 1913.)
(Wester and Bruins, 1914.)
(Baroni and Barlinetto, 1911.)
COLCHICINE
262
COLCHICINE C22H25N06.
SOLUBILITY IN SEVERAL SOLVENTS.
(Mliller, 1903; U. S. P.)
Gms.
Solvent.
Solvent.
Gms.
Water
Ether
sat. with H2O
18-22
25
80
82
18-22
25
1 8-2 2
per 100 Gms.
Solvent.
9.6
4-5
0.13
0.64
0.18
Water sat. with Ether 18-22
Benzene 18-22
Benzene 25
Chloroform 18-22
Carbon Tetrachloride 18-22
Ethyl Acetate 18-22
Petroleum Ether 18-22
per 100 Gms.
Solvent.
12.05
0.94
I -IS
IOO+
O.I2
'•34
0.06
Beilstein.
COLCHICINE SALTS.
Name.
Formula.
Solvent.
Colchicine lodohydrate C22H25NO6.HI Water
Iso Colcnicine lodohydrate
Gms. Salt
per Liter
Sat. Sol.
30
30
Authority.
(Pfannl, 1911.)
0.84
3-86
o . 083 (Jensen, 1913.)
0.007 "
COLLIDINE (2.4.6 Trimethyl Pyridine) C6H2N(CH8)8.
SOLUBILITY IN WATER.
(Rothmund, 1898.)
Gms. Collidine per 100 Gms.
Aq. Layer. Collidine Layer.
5.7 crit. t. 17.20
7.82 41.66
54.92
62.80
Gms. Collidine per 100 Gms.
10
20
30
40
60
3.42
2.51
1.93
1.76
70.03
80.19
Aq. Layer.
Collidine Layer.
80
i-73
86.12
100
i!78
88.07
120
1.82
88.98
I4O
2.19
89.10
160
2-93
87.2
180
3-67
...
COLLIDINE (1.3.5 Trimethyl Pyridine) C6H2N(CH3)3.
DISTRIBUTION BETWEEN WATER AND TOLUENE.
(Hantzsch and Vagt, 1901.)
G. Mols. Collidine per Liter.
G. Mols. Collidine per Liter.
t°.
H20 Layer.
Toluene
Layer.
Dist. Coef.
t°.
H2O Layer
Toluene
Layer.
Dist. Coef.
o
0.0035
0.0580
0.0603
50
0.0017
0.0596
0.0285
10
O.OO26
0.0587
0.0443
70
O.OOI5
0.0597
0.0251
20
O.OO22
0.0588
0.0374
90
0.0013
0.0598
0.0218
30
0.0020
0.0594
0.0337
CONGO RED [C6H4.N:N.CioH6(NH2)SO3Na]2.
100 gms. H2Q dissolve n.6 gms. congo red at 2O°-25°. (Dehn, 1917.)
100 gms. pyridine dissolve 0.29 gm. congo red at 20-25°.
100 gms. aq. 50% pyridine dissolve 7.32 gms. congo red at 20-25°. "
CONIINE (aPropyl Piperidine) C8HnN.
100 gms. H2O dissolve 1.83 gms. coniine at 20°. (Zalai, 1910.)
COPPER ACETATE Cu(C2H3O2)2H2O.
100 gms. glycerol (d^ = 1.256 = 96%) dissolve 10 gms. copper acetate at
I5°-l6°. (Ossendowski, 1907.)
263 COPPER ACETATE
SOLUBILITY OF ANHYDROUS COPPER ACETATE IN PYRIDINE.
(Mathews and Benger, 1914.)
t°. per 100 Gms. Solid Phase. t°. per 100 Gms. Solid Phase
Sat. Sol. Sat. Sol.
— 1 1. 6 0.37 CutQHsOz^CsHsN 45.2 4.17
+ 2 0.6 " 34.8 3.75 Cu(C5H302)2.CsH6N
13 I-°3 55-7 4-13
26.45 Z-6I 64-3 4.48 "
37-4 2.83 " 76.2 4.83
41.9 3.12 83.3 5.40
43-2 3-39 95-4 6.31
Transition point = 44.7°.
COPPER ^BROMIDE (ous) Cu2Br2.
SOLUBILITY OF CUPROUS BROMIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
BROMIDE AT i8°-2O°.
(Bodlander and Storbeck, 1902.)
Millimols per Liter. Grams per Liter.
KBr.
Total Cu.
Total Br. Cu (ic).
Cu (ous).
KBr.
Total Cu.
Cu (ic).
Cu (ous).
0
O
•3157
0.4320 o
.2096
0.1061
0
O.O2OI
O
•0133
0.0067
25
0
.119
0
.012
0.107
2
.98
O.OO76
0
.0007
0.0068
40
0.200
.' . . 0
•013
0.187
4
.76
O.OI27
0
.0007
O.OII9
60
O
.310
0
•025
0.285
7
•15
O.OI97
0
.0015
O.OlSl
80
0
•423
0
.012
0.411
9
•53
O.0266
0
.0007
O.026l
IOO
0
•584
. . .
0.584
ii
.91
0.0371
. . .
0.0371
120
0
•693
. . .
0.693
14
.29
0.0441
0.0441
500
8
.719
. . .
8.719
59
•55
0-5540
0.5540
loo gms. acetonitrile dissolve 3.86 gms. Cu2Br2 at 18°. ' (Naumann and Schier, 1914.)
Freezing-point lowering data for mixture of CuBr + KBr are given by de
Cesaris, 1911.
COPPER BROMIDE (ic) CuBr2.
IOO gms. acetonitrile dissolve 24.43 £ms' CuBr2 at 18°. (Naumann and Schier, 1914.)
ioo gms. 95% formic acid dissolve 0.16 gm. CuBr2 at 21°. (Aschan, 1913.)
COPPER CARBONATE Basic.
SOLUBILITY IN AQUEOUS CO2 SOLUTIONS AT 30°.
(Free, 1908.)
Aq. 0.5 n Na2COs and 0.5 n CuSCX were mixed and the precipitate washed and
suspended in H2O containing CO2 at a pressure slightly above atmospheric, for
3 days. The filtered precipitate was kept in water ready for use. In the fresh
condition or dried, the molecular ratio of the constituents was found to be iCuO:
0.515 CO2: 0.61 H2O. For the solubility determinations, about 2 gms. of the
precipitate were suspended in 600 cc. of H2O and CO2 passed in to the desired
concentration. The mixture was shaken frequently for 3 days. The total COg
in the sat. solution was determined and the free CO2 calc. by difference, assuming
that the amount combined to the Cu was in the molecular ratio 2CuO:iCO2.
Parts per Million. Parts per Million.
Free CO2. Metallic Cu. Free CO2. Metallic Cii.
o = pure H^O i . 5 859 28
157 8.3 961 31
277 13-7 1158 33-7
348 17 1224 34.8
743 25.7 1268-1549 35-3-39-7*
* Saturated with CO2 at i + atmosphere.
Results practically identical with the above were obtained for a NaCl solu-
tion containing ioo parts per million. Data for other concentrations of NaCl
and for other salts are also given. Salts with a common ion depress the solubil-
ity. Those with no common ion increase it slightly. A recalculation of the
results of Free is given by Seyler (1908).
COPPER CARBONATE 264
SOLUBILITY OF MIXTURES OF COPPER CARBONATE AND POTASSIUM
CARBONATE IN WATER AT 25°.
(Wood and Jones, 1907-08.)
ioo gms. H2O dissolve 3.15 gms. CuCO3 + 105 gms. K2CO3 at 25° when the
solid phase in contact with the solution is CuCO3.K2CO3 + K2CO3.
Additional points on the curves were determined but the analytical data are
not given. The following approximate values were read from the curve for the
double salt, CuCO3.K2CO3:
Gms. per ioo Gms. H2O.
, • —• % Solid Phase.
K2CO3. CuCO3.
105 3.15 KgCOrf CuCO3.K2CO3
.100 3.20 CuCO3.K2CO3
90 3.40
85 3-6o
The triple point for double salt + CuCO3 could not be determined since
CuCO3 is not capable of existing alone and decomposes into CO2 + Cu(OH)a.
COPPER CHLORATE (ic) Cu(ClO3)2.4H2O.
SOLUBILITY IN WATER.
(Meusser, 1902.)
Gms. Mols. Gms. Mols.
t°. Cu(ClO3)2 Cu(ClO3)2 Solid Phase. t°. ' Cu(ClO3)2 Cu(ClO3)2 Solid Phase,
per ioo Gms. per ioo Mols. per ioo Gms. per ioo Mols. ^
Solutions. H2O. Solutions. H26.
-12 30.53 3.43 Ice l8 62.17 12.84 CuCClO,),.^©
-3i 54-59 9-39 Cu(ClO3)2.4H2O 45 66.17 15.28
-21 57.12 10.41 " 59.6 69.42 17.73 "
-f 0.8 58.51 11.02 ." 71 76.9 25.57 1
Density of solution saturated at 18° = 1.695.
COPPER CHLORIDE (ic) CuCl2.2H2O.
SOLUBILITY IN WATER.
(Reicher and Deventer," 1890; see also Etard, 1894.)
Gms. CuCl2 Gms. CuCl2 Gms. CuClj
t°. per ioo Gms. t°. per ioo Gms. t°. per ioo Gms.
Solution. Solution. Solution.
— 40 Eutec. 36.3 20 43.5 50 46.65
o 41.4 25 44 60 47.7
10 42.45 30 44.55 80 49.8
17 43-°6 40 45-6 ioo 51.9
Density of solution saturated at o° = 1.511, at 17.5° = 1.579.
ioo gms. sat. solution in water contain 43.95 gms. CuCl2 at 30°, solid phase,
CuCl2.2H2O. (Schreinemakers, 1910.)
COPPER CHLORIDE (ous) CuCl.
ioo gms. H2O dissolve 1.52 gms. CuCl at 25°. (Noss, 1912.)
SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID CONTAINING CuCl2 AT 25°.
(Poma, 1909, 1910.)
Results for i n HC1. Results for 2 n HC1. Results for 4 n HC1.
Mols. per Liter. Mols. per Liter. Mols. per Liter.
CuCl, •
Added.
CuCl2+CuCl. Phase.
Added. CuCl2+CuCl. Phase. C
dded. CuCla+CuCl.
SOlld
. Phaser
0
0.0862 CuCl
0
o
. 2365 CuCl
0
0
.7704
CuCl
0
.1
0.2017
O
.094
0
.3528 "
0
•095
0
.9044
"
0
.2
0.3256 «
o
.188
0
.4766 "
0
.189
I
.0370
M
0
•4
0.5707 «
0
• 235
0
•5385 "
o
•379
I
.3040
"
o
• 5
0.6924
o
.282
0
.6038 "
0
•473
I
.4380
«
265
COPPER CHLORIDE
SOLUBILITY OP CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OP HYDRO-
CHLORIC ACID.
(Engel — Ibid. [6] 17. 372, '89; Compt. rend. 121, 529, '95.)
Milligram Mols. jjer 10 cc. Sol.
iCu2Cl2.
HCl.
Results at o°.
o-475
8-975
i-5
17-5
2.9
26.O
4-5
34-5
8.25
47-8
15-5
68.5
104.0
Results at
i5°-i6°.
7-4
54-4
10.8
68.9
12.8
75-o
16 o
92.0
Sp. Gr. of
Solutions. '
Gms. per^ioo cc. Sol.
'Cu2Cl2/ HCL
Cms, per 100 Cms. Sol.
' HCL
I
•05
0.471
0
•327
o
.448
0
.312
I
.049
i
.486
0
.638
i
.418
0
.608
I
.065
2
.872
0
.948
2
.697
0
•932
I
.080
4
•457
I
•257
4
.127
I
.!64
I
•135
8
.172
I
•743
7
.199
i
I
.261
15
•7
2
•497
12
.46
i
^80
I
•345
32
.68
3
.827
24
•30
2
•845
I
.19
7
•33
I
•983
6
•159
I
.666
I
.27
10
.69
2
•5"
8
.422
I
•977
I
.29
12
.68
2
•734
9
.826
2
.119
I
•38
J5
.84
3
•346
ii
.48
2
•424
SOLUBILITY OF CUPRIC CHLORIDE IN AQUEOUS SOLUTIONS OP HYDRO-
CHLORIC ACID AT o°.
(Engel — Ann. chim. phys. [6] 17, 351, '89.)
Milligram Mols. per 10 cc. Sol. Sp Gr. of Gms. per 100 cc. Sol. Gms. per 100 Gms. Sol.
iCud2.
HCl. Solutions.
CuCl2.
HCl.
CuCl2.
HCI:
91
•75
O
1.49
61
.70
o.
0
41
• 41
o.o
86
.8
4
•5 *-475
58
•37
I.
64
39
•58
1 .11
83
.2
7
.8
.458
55
•95
2.
84
38
•37
1 .95
79
•35
10
•5
•435
53
•37
3-
83
37
.19
2.67
68
•4
20
•25
•389
46
.01
7-
38
33
.11
50
• o
37
•3*9
33
.62
13-
67
25
•5o
10.37
22
.8
70
•25
.231
15
•33
25-
61
12
.46
20.80
23
•5
102
.288
.81
37-
36
12
.27
29.00
26
•7
128
• O
•323
17
.96
46.
66
13
•57
35 -26
29
• o
Sat
.HCl
COPPER CHLORIDE, AMMONIUM CHLORIDE MIXTURES IN AQUEOUS
SOLUTION AT 30°.
(Meerburg — Z. anorg. Chem. 45, 3, '05.)
Grams per 100
Gms. Sat. Solution.
CuCl2.
0
NEUCl.'
29-5
28.6
3-6
10.5
25-9
I6.5
19.9
9-4
29.4
4-9
41.4
2.1
43-2
2-0
43-9
0
Grams per 100
Gms. Solid Phase.
'CuCl2.
6.0
37-o
21.7
28.5
35-i
43-1
48.2
34-9
23-1
18.4
15-3
13-3
6.6
Solid Phase.
NH^Cl
NH«C1 + CuCl2.2NH4Cl.2H2O
Cud8.2NH4Cl.aH20 + Cud2.iH,O
Additional determinations for the ammonia end of this system at 25° are
given by Foote, 1912.
COPPER CHLORIDE
266
COPPER AMMONIUM CHLORIDE CuCl2.2NH4C1.2H2O.
•io. s
-10.8
•ii
•io
o
12
20
per 100 Gms.
Solution.
3.87
2O. 12
20.3
20.46
22.O2
24.26
25-95
SOLUBILITY .IN WATER.
(Meerburg, 1905.)
Solid Phase.
Ice
<
Ice+CuCl2.2NH4C1.2H2O
CuCl,.2NH4C1.2H2O
30
40
50
60
70
80
Gms.
CuCl2.2NH4Cl
per 100 Gms.
Solution.
27.70
30.47
33-24
36.13
39-35
43.36
Solid Phase.
.SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OP CUPRIC
SULFATE AT ABOUT 2O°.
(Bodlander and Storbeck, 1902.)
Millimols per Liter.
Grams per Liter.
CuSO4.
Total Cu.
Total Cl.
Cu (ic).
Cu (ous).
CuSCv
Total Cu.
Total Cl.
Cu(ic).
Cu (ous).
o
2
.880
5-312
2.25$
O.622
O
0.183
O.lSS
0.143
' 0.040"
0.987
3
.602
4.908
3-145
0-457
o.
158
0.229
0.174
O.2OO
0.029
1-975
4
553
4.687
4-I3I
0.422
o.
315
0.290
0.166
0.263
0.027
2.962
5
193
4.256
4.625
0.509
o.
473
0.330
0.151
o. 292
0.032
4.937
7
276
4.329
6.546
0.730
0.
788
0.463
0.154
0.4l6
o . 046
SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF
POTASSIUM CHLORIDE AT ABOUT 20°.
(Bodlander and Storbeck, 1902.)
Millimols per Liter.
Grams per Liter.
KC1.
Total Cu.
Total Cl.
Cu (ic).
Cu (ous).
KC1.
Total Cu.
Total Cl.
Cu (ic).
Cu (ous).
0
2
851
5.416
2.222
0.629
0
o.
181
0.193
0.141
O.O4O
2.
5 i
955
6.015
I.42I
0-534
0.186
0.124
0.213
0.090
0.034
5
i
,522
7.525
1.008
0.5H
0-373
o.
097
0.267
0.069
0.033
10
i
.236
"•735
0-475
0.761
0.746
o.
079
0.416
0.030
0.048
20
i
,446
21.356
0.324
1. 122
1.492
o.
092
0-759
O.O2I
O.O7I
50
2
,411
notdet.
0.1088
2.302
3-730
o.
153
not det.
O.OO7
0.146
IOO
4
,702
«
O
4.702
7.460
0.
299
tt
O
0.299
2OO
9
485
M
O
9-485
14.920
0.
603
t(
0
0.603
1000
97
«
O
97
74.60
6.
170
u
0
6.170
2000
384
t(
0
384
149.2
24-
42
it
0
24.420
The results in the 3d, 7th, 8th and last line of this table are at 16°.
SOLUBILITY OF COPPER CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE.
(Hunt, 1870.)
Gms. CuClg per too cc. Solution of:
f.
Sat. NaCl.
iS%NaCl.
S%NaCL
II
8-9
3-6
40
11.9
6
I.I
90
16.9
10.3
2.6
267
COPPER CHLORIDE
SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF FERROUS
CHLORIDE AT 21.5° AND VICE VERSA.
(Kremann and Noss, 1912.)
In order to ascertain the composition of the solid phase, the experiment was
made by mixing together weighed amounts of H2O, CuCl and FeCl2 and agi-
tating in a thermostat at constant temperature. A weighed portion of the
clear saturated solution in each case was analyzed and the composition of the
solid phase calculated by difference.
Cms. per 100 Cms. H2O.
FeCl2.
CuCl. '
O
i-53
6.02
i-33
11.62
i. 80
16.30
3-n
26.30
7.12
29-35
8.06
33-12
9-S6
Solid Phase.
CuCl
M
Gms. per 100 Cms. H2O.
FeCl2.
CuCl. "
43-75
12.42
CuCl
54
17.04
«
66.40
21.6
u
73-20
23.20
71.90
21.65
F(
69.30
11.9
65.10
O
Solid Phase.
+FeCl2.4H20
FeCl2.4H20
SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 26.5° AND VICE VERSA.
(Kremann and Noss, 1912.)
(See remarks above.)
'NaCl.
0
10.8
CuCl.'
i-55
OUJ1U. i IltlbC.
CuCl
20.7
27
36.48
7-30
40.60
49.10
M
Gms. per 100 Gms. H2O.
Solid Phase.
' NaCl.
CuCl. '
44.14
57-21
CuCl
55-io
44.10
NaCl
56.80
41.70
"
50.90
18.70
u
SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AT 22° AND VICE VERSA.
(Bronsted, 1912.)
Gms. per 100 Gms. _ ,.
Sat. Sol. Solid
Gms. per 100 Gms. _ ...
Sat-Sol. lohd
Gms. per TOO Gms.
Sat. Sol.
Solid
Phase.
KC1.
CuCl.'
' KC1.
CuCl.
' KC1.
CuCl.
3-87
0
.115 CuCl
21
.64
13
.32 CuCl
24,
04
4
•53
CuCl.aKCl
6.56
0
•405 "
23
.84
17
-23
25
03
3
.14
"
8.24
O
.861 "
25
.24
21
•47
26
,28
a
.20
"
n-33
2
.19 "
23
.87
15
.48 CuCLaKCl
27
,06
i
.60
"
I5-30
4
.80 "
23
•57
13
•99
26
.68
-i
.21
KC1
17-47
7
.19 "
23
II
•39
26
32
0
-58
"
20.31
10
.21 "
23
-49
7
•35
25
.68
0
**
COPPER CHLORIDE 268
SOLUBILITY OF CUPRIC CHLORIDE IN AQUEOUS SOLUTIONS OF MERCURIC
CHLORIDE AT 35° AND VICE VERSA.
(Schreinemakers and Thonus, 1912.)
' HgCl2.
CuCl2.
auiiu r iia.se.
HgCl2.
CuCl2. "
ooiiu rnase.
O
44-47
CuCl2.2H2O
52-54
18.46
HgCl2
21.03
33-5
«
52.81
18.06
u
37-30
26.07
tt
51.03
14-73
((
44-47
23-31
tt
49-50
5-94
It
50-47
21 .50
" +HgCl2
23.87
2.64
tl
52-44
19.40
HgCl2
8.51'
0
tt
SOLUBILITY OF COPPER CHLORIDE AND POTASSIUM CHLORIDE DOUBLE
SALTS AND MIXTURES IN WATER.
(Meyerhoffer — Z. physik. Chem. 5, 102, '90.)
Cl per i Gram Solution. Mols.per iooMols.H2O.
* Solid
Phase.
CuCl2.2KC1.2H20 + KCl
CuCl2.KCl + KC1
CuCl2.2KC1.2H2O + CuCl2.2H2O
«
CuCl2.KCl + CuCl2.2H2O
ii
CuCl2.2KC1.2H2O + CuCl2.KCl
CuCl2JCCl
SOLUBILITY OF CUPRIC CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 30° AND VICE VERSA.
(Schreinemakers and de Baat, 1908-09.)
Gms. per 100 Gms. Sat. Sol. Gms. per TOO Gms. Sat. Sol.
, ^. • — — — > Solid Phase. . — ; • — — > Solid Phase.
MaCl. CuCl2. NaCl. CuCl2.
o 43-95 CuCl2.2H2O 12.25 32.40 NaCl
3.10 41.14 13.54 28.64
4.28 41.06 15-40 23.72
6.41 39.40 " 18.44 16.98 "
10.25 36.86 " +NaCl 20.61 11.03
12.02 32.38 NaCl 26.47 ° "
t<>.
Present as
CuCl2.
Present as
KC1.
CuCb.
KCl.
39-4
0.120
0.107
5.56
9-93
49.9
0.129
O.II5
6-39
11.4
60.4
0.142
0.125
7.71
13.6
79.1
0.168
O.I42
n. i
18.8
0.188
0.154
14.9
24.4
93-7
0.194
0.156
16.2
26.0
98.8
0.197
O.l62
17-5
28.7
o
0.214
O-02I
9.84
i-94
39-6
0.232
O.O49
12.9
5-44
50.1
0.233
0.059
13-7
6.90
0.241
0.062
14.8
7-63
60.2
0.246
O-o66
15-8
8-49
72.6
0-255
0.063
16.8
8-35
64.2
14.9
ii. 6
72-5
...
...
14.8
15.0
26$
: COPPER CHLORIDE
SOLUBILITY OF CUPRIC CHLORIDE? itf AQUEOUS ALCOHOL AT^II.S".
(Bodtker, 1897.)
10 gms. of CuCl22H2O and the indicated amounts of CuCl2 were added to
20 cc. portions of alcohol. The solutions shaken two hoursjand 5 cc. portions
withdrawn.
Vol. %
Gms. CuCl2
Gms. per 5
cc. Solution. '
Vol.
%
Gms. CuClj
Gms. per 5 cc.
Solution.
Alcohol.
Added."
' H2O.
CuCl2. "
Alco]
hoi.
Added. ,
> H20.
CuCl2. "
89.3
o
0.794
LI37
99
•3
0.223
0.330
I-29S
92.3
o
0.648
1.090
99
•3
0.887
0.247
1.639
96.3
0
0.478
1.116
99
•3
I.S40
0.191
2.086
99-3
o
0.369
1.208
99
•3
1-957
0.164
2.400
SOLUBILITY OF CUPRIC CHLORIDE IN SEVERAL SOLVENTS.
(Etard — Ann. chim. phys. [7] 2, 564, '94; de Bruyn — Z. physik. Chem. 10, 783, '92; de Coninck —
Compt.rend. 131, 59, 'oo; St. von Laszczynski — Ber. 27, 2285, '94.)
Grams CuCl2 per 100 Grams Sat. Solution at:
ooiveni.
0°.
15°.
20°.
40°.
80°.
Methyl Alcohol
36
40.5 (deB.)
36.5
37-o
Ethyl Alcohol
32
35.0 (deB.)
35-7
39-0
Propyl Alcohol
29
30-5
30-5
. . .
Iso Propyl Alcohol
. . .
16.0
30.0
n Butyl Alcohol
1^
. . .
J5-3
16.0
16.5
Allyl Alcohol
23
. . .
23.0
. . .
Ethyl Formate
10
9.0
8.0
Ethyl Acetate
. . .
...
3-0
2-5
i.3(720)
Acetone (abs.)
8.86*
8.92f
2.88
(18°) ...
1.40(56°)
Acetone (80%)
. . .
18.9$
Ether
0.043 (IJ°)
o.n
* (CuCl2.2 Aq.)
t(CuCl2.2Aq.)
* (23° CuCl2.2 Aq.)
For the solubility of cupric chloride in mixtures of a number of
organic solvents, see de Coninck.
Gms.
Solvent. V. g^T
Sat. Sol.
Acetonitrile 18 1.57
Ethyl Acetate 18 0.4
Methyl Acetate 18 0.55
Sp. Gr.
Sat. Sol.
Authority.
(Naumann and Schier, 1914.)
0.9055 (Naumann, 1904.)
O . 939 (Naumann, 1909.)
AnhydrOUS Hydrazine Ord. temp. 5 (decomp.) . . . (Welsh and Broderson, 1915.)
SOLUBILITY OF CUPROUS CHLORIDE IN ACETONITRILE. (Naumann and Schier, 1914.)
loo gms. acetonitrile of boiling point 81.6° dissolve 13.33 gms« CuCl at 18°.
SOLUBILITY OF CUPRIC CHLORIDE IN PYRIDINE.
:(Mathews and^Spero, 1917.)
Gms.
to CuCl2 per
100 Gms.
Sat. Sol.
0.140
0.195
0.295
— 12. 1
— IO
— 8.9 tr. pt. 0.270
+ 2 0.275
10 0.293
25 0.348
35 0.382
Gms.
Solid Phase.
t°
CuCl2 per
Solid Phase.
too Gms.
Sat. Sol.
:i,.6C5HBN
45
0.422
CuClj-aCjHjN
53
0-493
it
(unstable)
60
0.565
" (unstable)
+CuCl2.2C5H6N
62
0.616
" "
CuCl2.2C6H5N
58 tr. pt.
. . .
" +2CUC1J.3C5HSN
"
63
0-543
2CUC12.3C5H6N
(i
75
0.631
«
M
95
0.917
M
COPPER CHLORIDE 270
DISTRIBUTION OF CUPRIC CHLORIDE BETWEEN AQ. HC1 AND ETHER
When i gm. of copper as chloride is dissolved in 100 cc. of 10% HC1 and shaken
with loo cc. of ether, 0.05% of the metal enters the ethereal layer. (Mylius, 1911.)
COPPER Ammonium CHLORIDE CuCl2.NH4Cl.
SOLUBILITY IN ABSOLUTE ALCOHOL AT 25°. (Foote and Walden, 1911.)
Gms. per 100 Gms. Sat. Sol.
— • Solid Phase.
4.7 not det. NH4C1+ CuCl2.]
6.45 " CuCl2.NH4Cl
12.90
34-7 " +CuCl2.C2H5OH
COPPER Potassium CHLORIDE CuCl2.KCl.
SOLUBILITY IN ABSOLUTE ALCOHOL *ANDJN ACETONE AT 25°. (Foote and Walden, 191 1)
In Absolute Alcohol. In Acetone.
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
_ -. " ^7- . Solid Phase. TT-rr " — TTTT, • Solid Phase.
CuCl2. KC1. CuCl2. KC1.
1.40 0.28 KCl+CuCl2.KCl 0.34 0.38 KCl+CuCl2.KCl
2.15 not. det. Cud2.KCi 0.48 not det. CuCi2.Kd
5.25 " «• 1.50
30.16 " 2.06
34.45 0.21 " H-CuClz.QHBOH 2.40 0.27 " +CuCl2.C3H«O
33.97 O CuCl,.CfH,OH
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures of cuprous chloride and other chlorides.
CuCl + CuCl2 (Sandonnini, 1912 (a)).
+ FeCls (Hermann, 1911.)
+ PbCl2
-j- LiCl (Sandonnini, 1911, 1914; Korreng, 1914.)
-\- RbCl (Sandonnini, 1914; Sandonnini and Aureggi, 1912.)
+ AgCl (Sandonnini, 1911, 1914; Poma and Gabbi, 1911, 1912.)
-j- KC1 (Sandonnini, 1911,1914; Korreng, 1914; Sackur, 1913; Poma and Gabbi, 1911, 1912.)
+ NaCl (Sandonnini, 1911, 1914; Korreng, 1914; Sackur, 1913; de Cesari, 1911.)
+ T1C1 (Sandonnini, 1911, 1914.)
+ SnCl2 (Hermann, 1911.)
+ ZnCl2
Freezing-point lowering data for mixtures of CuCl + Cu2O and CuCl + Cu2S
are given by Truthe, 1912.
COPPER Potassium CITRATE CuK4[(COOCH2)2C(OH)COO]2.
100 cc. sat. solution in H2O contain 43.3 gms. of the salt at 10°. (Pickering, 1915.)
COPPER CYANIDE (ous) Cu2(CN)2.
Freezing-point data for Cu2(CN)2 + KCN and Cu2(CN)2 + NaCN are given
by Truthe (1912).
COPPER HYDROXIDE (ic) Cu(OH)2.
SOLUBILITY IN AQUEOUS SOLUTIONS OF AMMONIA AT 18°. (Dawson, 1909.)
Mols. NH3 per Gm. Atoms Cu per Mols. NH3 per Gm. Atoms Cu per
Liter. Liter. Liter. Liter.
0.2 0.00054 3 0.0548
0.5 0.0033 4 0.0784
1 0.0109 5 0.1041
1.5 0.0204 6 0.1254
2 0.0314 8 0.1599
2.5 0.0442 9.96 0.1787
Three series of results at 25°, somewhat higher than the above, are given by
Bonsdorff, 1904.
Data showing the effect of increasing amounts of (NH4)2SO4, Ba(OH)2, NaOH
and of Na2SO4 upon the solubility of cupric hydroxide in aqueous ammonia
solution at 18°, are given by Dawson, 1909 a.
271
COPPER IODATK
COPPER IODATE (ic) Cu(IO3)2H2O.
One liter sat. aqueous solution contains 1.36 gms. Cu(I03)2 at 25°, determined
by measurement of single potential differences against a o.i n calomel electrode.
(Spencer, 1913.)
COPPER IODIDE (ic) CuI2.
One liter sat. aqueous solution contains 11.07 gms. CuI2 at 20°.
(Fedotieff, ign-ia.)
COPPER IODIDE (ous) Cu2I2.
SOLUBILITY OF CUPROUS IODIDE IN AQUEOUS SOLUTIONS OF AMMONIUM
BROMIDE AND OF POTASSIUM BROMIDE.
(Kohn, 1909; Kohn, and Klein, 1912.)
Results for Aq. NH4Br at 20°. Results for Aq. KBr Solutions.
Normality Gms. Cu2I2 Normality Gms. Cu2I2 Normality Gms. Cu2I,
NHiBr per 1000 cc. t°. of KBr per 1000 cc. t°.
Sol. Sat. Sol. Sol. Sat. Sol.
2 1.9068 19.5 2 1.467 23
3 3-6540 24 2 1.558 22
4 6.0588 19.5 3 3.409 22
of KBr per 1000 Gms.
Sol. Sat. Sol.
3-595
7.126
6.977
SOLUBILITY OF CUPROUS IODIDE IN AQUEOUS SOLUTIONS OF IODINE AT 20°
AND VICE VERSA. (Fedotieff, 1910-11.)
Gms. per Liter. Solid Gms. per Liter.
Solid
Cu.
I. Phase. ' Cu.
i.
Phase.
0.285
0
.5848 Cul 0.964
5
.0854
Cul
0.482
I
•3053 "
.032
5
.6854
"
0.583
I
.9218 "
.090
6
.2816
"
0.678
2
•5573 "
.112
6
•5301
"
0.756
3
. 2042 "
.232
7
.6529
" +1
0.844
3
•9539 "
.040
6
.4440
I
0.898
4
•4359 " 0.898
5
•5941
"
Gms. per Liter.
Solid
Phase.
Cu. I.
0.748 4.7112 I
0.6o6 3.8562
0.448 2.9493 "
0.300 2.0689
0.159 I-2304 "
at o°= 0.925 5.4609 Cui+i
at 40°= i. 658 11.3658 "
_ Constant agitation and temperature. Iodine determined by thiosulfate titra-
tion; copper, electrolytically.
Additional data for the solubility of cuprous iodide in aqueous solutions of
iodine in presence of acids and salts at 25°, are given by Bray and MacKay
(1910). These authors state that cuprous iodide is difficultly soluble in water,
but in the presence of iodine a considerable amount dissolves, owing to the
formation of cupric iodide and tri-iodide.
100 gms. acetonitrile dissolve 3.52 gms. Cu2I2 at 18°. (Naumann and Schier, 1914.)
Freezing-point lowering data for mixtures of Cul + Agl are given by Quercigh, '14.
COPPER NITRATE (ic) Cu(NO3)2.
SOLUBILITY IN WATER.
Gms.
to Cu(N03)2
' per 100 Gms.
Mols.
Cu(NO3)2
per too
Solid Phase.
Solution.
•Mols. H2O.
-23
36.08
5-42
Cu(NO3)2.9H2O
— 20
40.92
6-65
•
— 21
39-52
6.27
Cu(NO3)2.6H2O
0
45
7.87
M
+ 10
48.79
9-15
«
18
53-86
11.20
II
(Funk, 1900.)
Gms.
Mols.
r.
per 100 Urns. per
Solution. Mols. H2O.
scud Ph-
55.58
Cu(NOJ),.3H10
20
26.4
25
40
60
80
II4-5
Density of solution saturated at 18° = 1.681.
100 gms. H2O dissolve 127.4 gms. Cu(Np3)2at2O0,<f20sat. sol. = 1.688. (Fedotieff , 1911-12.)
Data for the solubility of copper nitrate in aq. ammonia solutions are given
by Stasevich, 1913. ,
Data for the solubility of copper nitrate in aq. solutions of copper sulfate
and of sodium nitrate at 20° are given by Massink, 1916 and 1917.
100 cc. anhydrous hydrazine dissolve I gm. copper nitrate, with decomposi-
tion, at room temp. (Welsh and Broderson, 1915.)
60. 01
6I.5I
64.17
67-5I
77-59
12
I6.7
14.4
15.2
17.2
2O
33-3
Cu(NO3)j.6H,O
COPPER OXALATE
272
COPPER OXALATE (ic) CuC2O4.£H2O.
One liter H2O dissolves 0.02364 gm. CuC2O4 at 25°, determined by the con-
ductivity method. (Schafer, 1905.)
COPPER OXIDE (ic) CuO.
SOLUBILITY IN AQUEOUS SOLUTIONS AT 25°.
(Jaeger, 1901.)
In Aq. HF + KF.
Gm. Atoms
Cu per Liter.
0.0356
0.06437
0.1442
In Aq. Hydrofluoric Acid.
Normality Gm. Atoms
Cu per Liter.
0.0307
O.II64
0.2494
0.388
0.463
In Aq. HN03 and CH3COOH.
ofHF.
0.12
0.28
o-57
i. 08
2.28
Normality
of HF.
Solvent.
i n CHaCOOH
i n HNO3
Gm. Atoms
Cu per Liter.
0.1677
0.4802
Cu determined electrolytically.
0.12
0.28
0-57
I. II O.
2.17 o.
COPPER OXIDE (ous) Cu2O.
SOLUBILITY IN AQUEOUS AMMONIUM SOLUTIONS AT 25°.
(Donnan and Thomas, 1911.)
The cuprous oxide was prepared by adding KOH solution to a mixture of
equal weights of CuSO4.sH2O and sucrose dissolved in water, until nearly all the
precipitate had redissolved. The solution was kept at 70° until the cuprous
oxide had separated. Two batches were prepared. The first, No. I, obtained
from the more dilute solution, was bulky and dark red in color, Cu = 88.62%.
The second, No. II, was bright red, Cu = 88.59%. The solubility determina-
tions were made with extreme care. A special apparatus was used. By means
of this, the constituents of the mixtures were introduced into the bottles in an
atmosphere of hydrogen and every precaution taken to prevent oxidation. The
bottles were sealed and rotated for 2-4 weeks at constant temperature. In
case the slightest tinge of blue developed in a bottle (indicating oxidation), it
was rejected.
Results for Preparation No. I. Results for Preparation No. II.
Gms. per 1000 Gms. Sol. Mols. per 1000 Gms. Sol. Gms. per 1000 Gms. Sol. Mols. per 1000 Gms. Sol.
Cu.
NH3.
Cu.
NH3.
Cu.
NH3.
Cu.
NH3.
0-3593
3
.91
0
.00566
0.23
0.4229
7
.82
0
.00665
0.46
0.6869
13
•77
0
.01080
0.81
0.6678
8
.16
0
.01050
0.48
I.OI44
27
•°3
o
•01597
i-59
o . 9890
22
.61
o
•01555
i-33
I . 0462
32
.64
o
.01645
1.92
1.0494
28
•39
o
.01650
1.67
1.3229
68
.68
0
.02081
4.04
1.3528
54
•15
0
.02127
3-i9
1.4882
74
.12
0
.02340
4-36
I . 5048
72
.08
o
.02366
4.24
1-6313
98
•52
o
•02565
5-56
1.5963
78
.20
o
.02510
4.60
1.6981
122
.40
0
.02670
7.20
1-6555
102
•05
0
.02603
6
COPPER SULFATE CuSO4.sH2O.
SOLUBILITY IN WATER.
(Etard, 1894; Patrick and Aubert, 1874; at 15°, Cohen, 1903; at 25°, Trevor, 1891.)
Gms. CuSO4 per 100 Gms.
O
10
20
25
30
40
50
Solution.
12-5
I4.8
Water.
14.3
17-4
17.2
20.7
18.5
22.7
20
22.5
25
28.5
25
33-3
to
Gms. CuSO4 per 100 Gms.
•
Solution.
Water.
60
28.5
40
80
35-5
55
100
43
75-4
120
44
78.6
140
44-5
80.2
160
44
78.6
180
43
75-4
SO at
16° = 1.193.
(Greenish,
1902.)
Sp. gr. of sat. solution of CuSO4.sH2O in H2O at 16° = 1.193.
100 gms. sat. solution in H2O contain 20.32 gms. CuSO4at 30°. (Schreinemakers, 1910.)
273
COPPER SULFATE
SOLUBILITY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF AMMONIUM
SULFATE AT o°.
(Engel, 1886.)
Milligram Equiv. per
10 cc. Solution.
Sp. Gr. of
Grams per
too cc. Solution.
(NH4)2S04.
CuSO.
ions.
(NH4)2S04.
CuSO4.
0
18.52
I.I44
0
14.79
5-45
20.15
I.I90
3.61
16.09
7
10.5
1.108
4.63
8.38
7-4
9.1
1.099
4.90
7.26
8-45
6.425
I.08I5
5-59
5-13
n-35
3-7
I.07I
7.51
2.95
18.6
1.178
1.082
12.31
0.94
31-2
i
1.116
20.65
0.80
SOLUBILITY OF MIXTURES OF COPPER AMMONIUM SULFATE AND NICKEL
AMMONIUM SULFATE IN WATER AT i3°-i4°:
(Fock, 1897.)
CuSO4.(NH4)2SO4.6H2O + NiSO4.(NH4)2SO4.6H2O,
Mol. % in Solution.
Mols. per top Mols. H2O.
Mol. % in Solid Phase.
Cu Salt.
0
33-34
56-05
73.89
79-92
100
Ni Salt.
IOO
66.66
43-95
26.20
20.08
0
Cu Salt.
0
0.1476
0.2664
0.4165
0.4785
I-0350
Ni Salt."
0.521
0.295
o . 2089
0.1449
0.1202
O
Cu Salt.
0
10.29
30.59
52.23
78.80
IOO
Ni Salt.
IOO
89.71
69.41
47-77
21. 2O
0
SOLUBILITY OF MIXTURES OF COPPER AMMONIUM SULFATE AND ZINC
AMMONIUM SULFATE IN WATER AT i3°-i4°.
(Fock, 1897.)
CuSO4.(NH4)2SO4.6H2O + ZnSO4.(NH4)2SO4.6H2O.
Mol. % in Solution.
Mols. per 100 Mols. H2O.
Mol. % in Solid Phase.
' Cu. Salt
Zn Salt]
Cu Salt.
Zn Salt.
"Cu Salt.
Zn Salt.
4-97
95 .03
O.O422
0.8069
2-39
97.61
10.65
89-35
0.0666
0-5638
4-52
95-48
19.24
80.76
0.1218
0.5H5
9°-3
90.97
30.19
69.81
0.2130
0.4924
14.67
85-33
44-44
55-56
0.3216
0.4022
22.62
77.38
IOO
o
1-035
0
IOO
0
SOLUBILITY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF MAGNESIUM
SULFATE AT o°.
(Diacon. 1866.)
Gms. per 100 Gms. H2O.
CuSO4. MgSO4.
o 26.37
2.64 25.91
4-75 25.30
9.01 23 . 30 MgS04.6H,0+CuS04.sHzO
Solid Phase.
MgS04.6H20
Gms. per too Gms. H2O.
CuSCv
12.03
I3.6I
14.99
MgS04.
I5-67
8.64
O
Solid Phase.
CuS04.sH,0
COPPER SULFATB
274
SOLUBILITY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF COPPER
CHLORIDE AT 30°.
(Schreinemakers, 1910.)
Cms. per 100 Gms.
Sat. Sol.
CuSO4.
20.32
13.62
8.93
4-77
o
6.58
15.68
25.67
Solid Phase.
CuS04.5H2O
Gms. per 100 Gms.
Sat. Sol.
CuCl2.
39-48
42.62
43-25
43-95
CuS04.
3.21
2.90
I.I4
O
Solid Phase.
CuSO4.sH2O
"+CuCl2.2H2O
CuCl2.2H20
DATA FOR EQUILIBRIUM IN COMPLEX SYSTEMS CONTAINING COPPER SULFATE.
System. Authority.
CuSO4 + CuCl2 + (NH4)2SO4 + NH4C1 + H2O (Schreinemakers, 1910.)
" + " + K2SO4 + KC1 -f H2O (Schreinemakers and deBaat, 1914 a.)
" + " + Na2SO4 + NaCl + H2O (Schreinemakers, 1911.)
" + Li2SO4 + (NH4)2SO4 + H2O (Schreinemakers, 1909.)
SOLUBILITY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF LITHIUM
SULFATE AT 30°.
(Schreinemakers, 1908, 1909.)
Gms. per too Gms.
Sat. Sol.
'Li2S04.
O
3-54
6.08
11.94
I5-72
CuSO4.
20.32
17-59
16.10
13-55
12.14
Solid Phase.
CuSO4.5H2O
Gms.
>er loo Gms.
it. Sol.
Li2S04.
17.92
20-55
22.23
23-59
25.24
CuSO4.
II .04
IO.O5
6.41
3-39
o
Solid Phase.
CuSO4.5H2O
" +Li2SO4.H2O
Li2SO4.H2O
SOLUBILITY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF LITHIUM AND
OTHER CHLORIDES AT 25°.
(Herz, 1910.)
In Lithium
Chloride.
Gms. per 100 cc.
Sat. Sol.
In Potassium
Chloride.'
Gms. per 100 cc.
Sat. Sol.
In Rubidium
Chloride.
Gms. per 100 cc.
Sat. Sol.
In Sodium
Chloride.
Gms. per too cc.
Sat. Sol.
LiCl. CuS04.
3.10 20.06
5-93 18.78
12 17.03
KC1. CuS04.
4.19 23.89
8.75 24.92
17.50 29.03
' RbCl. CuS04,
o 22.34
13.22 25.02
. NaCl. CuSO4.
2.10 22.41
7.72 22.76
14.79 24.05
SOLUBILITY OF. COPPER POTASSIUM SULFATE CuK2(SO4)2.6H20 IN WATER AT 25°.
loo gms. H2O dissolve 11.14 Sms- CuK2(SO4)2. (Trevor, 1891.)
Additional data for the system Copper sulfate -f Potassium sulfate + H2O are
given by Meerburg, 1909.
Data for the solubility in water of mix-crystals of copper sulfate and man-
ganese sulfate at o° and 17°, and of copper sulfate and zinc sulfate at 12°, 18°,
25°i 35°» 40° and 45°, are given by Hollemann, 1905-06.
275
COPPER SULFATE
COPPER SULFATE, MANGANESE SULFATE, MIXED CRYSTALS AT 25°.
(Stortenbecker, 1900.)
Cms, per 100 Gms. HaO. Mols. per 100 Mols. H2O,
CuSCv MnSO4.
Tridinic Crystals with sH2O.
20.2
19.76
I3-65
ii. 61
9-39
6-47
o
3-69
St'S*
39-4i
46.77
53-39
58-93
o.o 61.83
Monoclinic Crystals with 7H2O.
9-39
6-47
o.o
46.77
53-39
Cu.
2.282
2.23
1-54
I-31
i. 06
o-73
0.34
o.o
i. 06
o-73
o.o
Mn.
O
0.44
3-76
5-59
6-37
7-03
7-375
5-58
6-37
8±*
Mol. % Cu
in Solution.
Mol. % Cu
in Crystals.
100
100
90-5
83.5
99-3
74.1
97-3
57-7
31-0
*l'.l
29.0
26.1
21.8
70.4
21.2
42.6
20.0
34-4
13-45*
22.9
15 .2*
10.27
10-5
4-6
4.9
2.31
2.15
o.o
IOO.O
20. o
10.27
4,6*
o.o
28.2
23-5
20.8
16.0
5-8*
100
* Indicates points of labil equilibrium.
COPPER SULFATE, ZINC SULFATE, MIXED CRYSTALS IN WATER AT 18°.
(Stortenbecker, 1897.)
Triclinic Crystals with
Monoclinic Crystals with 7H2O.
Rhombic Crystals with 7H2O.
Mols. per 100 Mols. H2O.
Mol. % Cu
Mol. % Cu
Cu.
Zn.
in Solution.
in Crystals.
2.28
0
100
100
-83
2.08
46.8
94.9
-41
3-60
28.1
.19
5-01
19.2
77-9
.86
3-36
36.2
40.4
.22
4-45
21-5
29-5-3I-9
.01
4.72
17.6
24.1-28.
0.82
5-03
14.0
19.0-22.
0.51
5-59
8.36
12.4-14-9
0.30
5-56
4.87
7.02
o.o
6.42
o.o
0
1.19
5.01
19.2
5.01
0.51
5-59
8.36
1.97
0.267
5-77
4.42
i-i5
o.o
5-94
o.o
0-00
COPPER SULFATE
276
SOLUBILITY OF COPPER SULFATE, SODIUM SULFATE MIXTURES IN WATER.
(Koppel, 1901-02; Massol and Maldes, 1901.)
Solid Phase.
CuS04.5H20+Na«SO4.ioH2O
CuSO4.NajSO<2H2O
CuS04.Na2S04.2H20+CuS04.sH20
Gms. per 100 Gms.
t»t Solution.
Mols. per 100 Mols.
H20.
" CuSO4.
NajSO,.
CuSO4.
NajSO4.
O
13.40
6.23
1.88
0.98
IO
14.90
9.46
2.23
1.56
15
15.18
11.64
2-34
2.02
17.7
14-34
13-34
2.24
2-34
23
14.36
12.76
2.23
2.21
40.15
13-73
12.26
2.10
2.10
17.7
14.99
I3-48
2-37
2-39
23
16.41
n-35
2-57
1.99
40.15
20.56
8
3-25
1.47
18
13-53
13.84
2.10
2.41
20
n-34
I5-70
I.76
2-73
25
6.28
21.20
0.98
3-70
30
2.607
28.38
0-43
5-2i
33-9
1-475
32.30
0.25
6.18
37-2
1-494
31.96
0.25
6.08
30
5-38
22.17
30.1
3 -69
25-37
30
i-57
32.09
«
CuS04.Na2S04.2H20 +increasing
Data tor the system copper sulfate, sodium sulfate, water, at 20° and 35*
are given by Massink, 1916, 1917.
SOLUBILITY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 0°. (Engel, 1887.)
Milligram
Eqvnv.
H,0.
per 10 Gms.
Sp. Gr. of
Solutions.
I.I44
Grams per 100 Grams
H20.
H2S04.
0
CuSO4.
18.6
H2S04.
0
cuso4:
14-85
4.14
14.6
17.9
19.6
I
I
-143
.158
2
7
•03
.16
14.29
15-65
54-2
56-25
71.8
12.4
8.06
7-75
5
I
I
I
I
.170
•195
.211
.224
15
26
27
35
.20
•57
•57
.2
9.90
6.43
6.19
3-99
SOLUBILITY OF
COPPER SULFATE IN AQUEOUS
AT 25°. (Bell and Taber, 1908;
SOLUTIONS
Foote, 1915.)
OF SULFURIC
ACID
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
CuSO4.sH20
< Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
CuSO4.3H2O+CuSO
CuS04.H20
H20
H2S04.
0
11.14
CuSO4.
18.47
12.62
H2S04.
55-72
61.79
CuS04.
2.13
o-95
25
36
42
47
49
•53
•77
.66
5
3
2
2
2
.92
•25
-63
•59
-83
M
" +CuSO4.sH2O
77
83
85
85
86
•93
.29
.46
.76
.04
0.17
0-15
0.19
0-43
0.40
u
If
" +CuS04
CuS04
50
54
•23
.78
2
2
.70
.19
CuSO4.3H2O
92
.70
0.19
277
COPPER SULFATE
SOLUBILITY OF COPPER SULFATE IN METHYL AND ETHYL ALCOHOL, ETC.
(de Bruyn, 1892; de Coninck, 1905.)
Solvent.
Methyl Alcohol Abs.
" 93-5%
" 50%
" " Abs.
Ethyl Alcohol Abs.
Glycol
Glycerol
Glycerol
95% Formic Acid
Anhy. Hydrazine
Cms, per ioo Gms. Solv. SOLUBILITY IN AQUEOUS
i8
18
18
3
3
14.6
15-5
15-16
CuS04. CuS04.sH20.
1.05 15.6
0-93
0.40
... 13.4
ALCOHOL AT 15°.
(Schiff, 1861.)
Alcohol
Gms. CuSO4.sH2O
per ioo g. Solvent.
IO
20
40
I.I
7-6*
30
36 . 3 (Ossendowski, 1907.)
15-3
3-2
0.25
ord. t. 2
* Per ioo gms. solution.
O'O5
. . . t
(Welsh and Broderson, 1915.)
t decomp.
Data for the solubility of copper sulfate in methyl alcohol are given' by Carrara
and Minozzi, 1897.
COPPER SULFIDE (ic) CuS.
1 One liter of water dissolves 0.00033 gm. CuS at 18°, determined by the conduc-
tivity method. (Weigel, 1906; see also Bruner and Zawadski, 1909.)
ioo cc. sat aq. sodium sulfide solution (of d = 1.225) dissolve 0.0032 gm. CuS.
(Holland, 1897.)
SOLUBILITY OF COPPER SULFIDE IN AQUEOUS SUGAR SOLUTIONS.
(Stolle, 1900.)
insolvent.
10
30
50
Gms. CuS p<
:r Liter of Aq. Sugar
1 Solution at:
17.5°-
0.5672
0.8632
0.9076
45°-
0-3659
0.7220
1.0589
75°. '
I-I34S
1.2033
I . 2809
COPPER SULFIDE (ous) Cu2S.
Freezing-point lowering data (solubility, see footnote, p. i) for mixtures of
Cu2S + Ag2S, Cu2S + PbS and Cu2S + ZnS are given by Friedrich, 1907-08.
Results for Cu2S + Sb2S3 are given by Chikashigi and Yamanchi, 1916. Data
for Cu2S + FeS are given by Shad and Bornemann, 1916.
COPPER SULFONATES.
100 gms. H2O dissolve 0.25 gm. copper 2-phenanthrene monosulfonate at 20°.
0^26 " " 10- "
COPPER TARTRATE CuC4O6H4.3H2O.
SOLUBILITY IN WATER.
(Cantoni and Zachoder, 1905.)
(Sandquist, 1912.)
t°.
Gms.
per ioo cc.
t°.
Gms.
CuC406H4.3H20
per ioo cc.
t°.
Gms.
CuC4OfH4.3H2O
per ioo cc.
Solution.
Solution.
Solution.
15
0.0197
40
0.1420
65
0.1767
20
0.0420
45
0.1708
70
0.1640
25
o . 0690
O.I92O
75
0.1566
30
o . 0890
55
0.2124
80
0.1440
35
0.1205
60
0.1970
85
0.1370
COPPER THIOCYANATE
278
NH3.
Cu(SCN)2.
0.79
2-45
1.98
4.08
2.50
5.11
4.26
5.96
5-35
6.22
6-39
6-59
9-93
7.98
16.55
11.24
21.47
15.22
COPPER THIOCYANATE (ic) Cu(SCN)2.
SOLUBILITY IN AQUEOUS AMMONIA SOLUTIONS AT 25° AND AT 40°.
(Horn, 1907.)
Results at 25°. , Results at 40°.
dv, Gms. per 100 Gms. Sat. Sol. ^.^ ^^^ Gms. per 100
Sat.
1.0082 0.70 2.4S Cu(SCN)2.2NH3
I.OI66
I .O2I3
I.OI7I 4.26 ^.Q6 Cu(SCN)2.4NH3
1.0151
1.0134
1.0070
0.9987
0.9985
COUMARIN C9H6O2.
100 gms. water dissolve o.oi gm. coumarin at 2O°-25°. (Dehn, 1917.)
" pyridine 87.7 gms.
50% aq. pyridine 60. i
" chloroform 49.4 " 25°. (Osaka, 1903-08.)
Freezing-point lowering data for mixtures of coumarin and sulfuric acid are
given by Kendall and Carpenter, 1914.
CRESOLS C6H4(OH)CH3 o, m and p.
SOLUBILITY OF EACH SEPARATELY IN WATER.
(At 20°, Vaubel, 1895; Sidgwick, Spurrell and Davies, 1915.)
Determinations by synthetic method; melting-point of o = 29.9°, of m = 4°,
of p = 33-8°. Triple point for o = 87 and 2.5 gms. per 100 gms. sat. sol. at
8°; triple point for p = 86 and 2 gms. per 100 gms. sat. sol. at 8.7°.
NH3.
Cu(SCN)2.
» ooiiu rnase.
0.94
2.81
Cu(SCN)2.2NH3
1.77
4.18
"
2-57
6.55
"
3-52
8.76
«
4-35
11.78
Cu(SCN)2.4NH3
5-50
12.07
"
7-58
12.99
«
13.98
16.58
"
18.02
19.76
•
Gms. per 100 Gms. Sat. Solution.
20
40
o Cresol.
2-45
3.08
m Cresol.
2.18
2.51
p Cresol.
1-94
2.26
50
60
3.22
3-40
2.72
2.98
2-43
2.69
70
80
90
3-74
4.22
4.80 •
3-35
4-43
3-03
3-52
4.16
100
5-30
5-47
5.10
no
< .80
5-SO
^0 Gms. per too Gms. Sat. Solution.
o Cresol.
m Cresol.
P Cresol.
120
6.22
7
6.58
I30
6.70
8.86
9
I4O
7.67
12.3
15-9
143.5 crit- *.
. . .
. . .
CO
147 crit. t.
00
150
II. I
160
23-7
162. 8 crit. t.
00
One liter aqueous I normal solution of the sodium salt of o cresol dissolves
7.57 gms. o cresol at 25°, 8.32 gms. at 40°, 9.84 gms. at 60° and 13.62 gms. at 80°
(Sidgwick, 1910.)
MISCIBILITY OF AQUEOUS ALKALINE SOLUTIONS OF m CRESOL WITH SEVERAL
ORGANIC COMPOUNDS INSOLUBLE IN WATER.
(Sheuble, 1907.)
To 5 cc. portions of aq. KOH solution (250 gms. per liter) were added the
given amounts of the aq. insoluble compound from a buret, and then the m cresol
dropwise, until solution occurred. Temp, not stated.
Composition of Homogeneous Solution.
cc. Aq. KOH.
Aq. Insol. Cmpd.
m Cresol.
5
2
CC.
(I
.64
gms,
.) Octyl Alcohol*
I
.1
gms.
5
5
tt
(4
.1
tt
) "
I
.8
tt
5
2
"
(i
•74
tt
) Toluene
4
•4
"
5
3
tt
(2
.61
it
\ a
5
.1
"
5
2
"
(I
.36
tt
) Heptane
6
•4
n
the normal secondary alcohol, the so-called capryl alcohol, CH3(CH2)sCH(OH)CHa.
279
CRESOL
DISTRIBUTION OF CRESOL BETWEEN WATER AND ETHER. (Vaubel, 1903.)
Composition of Solvent. Gms- ^jj 'm H2° ln Ether Layer.
200 cc. H20+ioo cc. Ether 0.0570 i .0760
200 cc. H2O+200 cc. Ether 0.0190 i .1144
FREEZING-POINT LOWERING DATA (Solubility, see footnote, p. i) FOR MIX-
TURES OF o, m AND p CRESOL (each determined separately) AND OTHER
COMPOUNDS.
Mixture. Authority.
o, m and p Cresol + Dimethylpyrone (Kendall, 1914.)
-j- Picric Acid (Kendall, 1916.)
" + Pyridine (Hatcher and Skirrow, 1917.)
0 and p + (Bramley, 1916.)
+ Sulfuric Acid (Kendall and Carpenter, 1914.)
4- Urea (Kremann, 1907.)
o, m and p ,
Trinitrocresol + Naphthalene
(Saposchinikow and Gelvich, 1903, 1904.)
CROTONIC ACIDS a. ^CHsCHrCHCOOH, 0 = HCH3C:CHCOOH.
FREEZING-POINT LOWERING DATA FOR MIXTURES OF CROTONIC ACIDS AND OF
CROTONIC ACID AND OTHER COMPOUNDS.
Mixture. Authority.
a Crotonic Acid + ft Crotonic Acid (Morrell and Hanson, 1904.)
" + Dimethylpyrone (Kendall, 1914.)
+ Sulfuric Acid
Chlorocrotonic Acid + Dimethylpyrone
" + Sulfuric Acid
(Kendall and Carpenter, 1914.)
(Kendall, 1914.)
(Kendall and Carpenter, 1914.)
Methyl CRYPTOPINES, A, B and C forms, C22H25O5N.
The solubilities of the three forms in benzene, determined by lowering of the
freezing-point, are: 5 gms. A form per liter at 5°, 30 gms. B form and no gms. C
form. (Sidgwick, 1915.)
CUMINIC ACID C3H7C6H4.COOH (p Isopropyl Benzole Acid).
SOLUBILITY IN WATER AT 25°. (Paul, 1894.)
looo cc. sat. solution contain 0.1519 gm. or 0.926 millimol cuminic acid.
PseudoCUMIDINE (CH3)3.C6H2.NH2 (s, 5 Amino, i. 2. 4, Trimethyl Benzene).
SOLUBILITY IN WATER.
(Lowenherz, 1898.)
t°. 19.4°. 23.7°. 28.7°.
Gms. \l/ Cumidine per liter H2O i . 198 i .330 i .498
CYANAMIDE CN.NH2.
SOLUBILITY IN WATER, DETERMINED BY FREEZING-POINT METHOD.
(Pratolongo, 1913.)
Gms. "
Gms.
fc° of Congealing.
CN.NH2 per
100 Gms.
Solid Phase.
Sat. Sol.
— 0.62
2.58
Ice
- 3.96
9.42
"
- 7.58
18.40 .
" .
— 12.72
30-9
<(
— i6.6Eutec.
37-8
" +CN.NH,
-15-6
38.75
CN.NH2
f of Congealing.
Sat. Sol.
-14-39
40.19
- 2.49
56.80
+14.50
77.20
25.6
87-I5
37-90
96.77
42.9
100
Solid
Phase.'
CN.NH,
Similajata forCN.NHi + urea and^CN.NHa + dicyandiamide are also' given.
DiCYANDIAMIDINE Perchlorate C2H6N4OHC1O4.
'"loo'gms. H2O dissolve 9.97 gms. of the salt at 17° (d sat. sol. = 1.039). (Carlson, 1910.;
CYANOGEN 280
CYANOGEN (CN)2.
SOLUBILITY IN WATER AND OTHER SOLVENTS.
(Berthelot, 1904.)
The determinations were made over mercury with exclusion of air. The
mercury was not attacked by the (CN)2. On account of polymerization, the
solubility increased with time of contact and amount of agitation of the mixture.
One volume of H2O at 30° dissolves 3.5 vols. (CN)2 after 2 hours, and 9.7 vols.
after 97 hours.
One volume of abs. alcohol at 20° dissolves 26 vols. (CN)2 immediately; 39
vols. after 4 hours; 89 vols. after 48 hrs. and 223 vols. after 4 days.
One volume glacial acetic acid dissolves 42 vols. of (CN)2 immediately and
50.5 vols. after 3 days.
One volume of chloroform dissolves about 19 vols. (CN)2 immediately and
29-30 vols. with time.
One volume of benzine finally dissolves 28 vols. (CN)2.
One volume of rectified turpentine dissolves 9-10 vols. of (CN)2.
One volume of ether dissolves 5 vols. (CN)2 at 20°. (Gay Lussac.)
CYCLOHEXANE (Hexamethylene, Hexahydrobenzene) CH2 < (CH2.CH2)2 >
CH2.
Freezing-point data (solubility, see footnote, p. i) for mixtures of cyclo-
hexane and ethylene bromide are given by Baud (i9i3b). Results for mix-
tures of cyclohexane and methyl alcohol are given by Lecat (1909). Results
for mixtures of cyclohexane and piperidine are given by Mascarelli and Con-
stantino (1909, 1910).
CYCLOHEXANOL (CH2)5.CHOH.
100 gms. H2O dissolve 5.67 gms. cyclohexanol at 11°. (de Forcrand, 1912.)
loo gms. cyclohexanol dissolve 11.27 Sms- H2O at 11°.
RECIPROCAL SOLUBILITY OF CYCLOHEXANOL AND WATER, DETERMINED BY
THE FREEZING-POINT METHOD.
(de Forcrand, 1912.)
Gm. (CH2)5.CHOH Gm. (CH2)5CHOH
t° of Solidification. per 100 Gms. t° of Solidification. per 100 Gms.
Mixture. Mixture.
+ 22.45 loo -57.4Eutec. 95-°3°
17.48 99-767 -43-2 93-I50
— 1.40 98.817 -33 91.962
—34.10 96.868 —18.50 90.980
-46.80 95-910 -14-58 9°-36
-55.70 95-I70 . -12.05 88.73
Freezing-point data for mixtures of cyclohexanol and phenol are given by
Mascarelli and Pestalozza, 1908, 1909.
CYCLOHEXANONE (CH2)6:CO.
Freezing-point data for mixtures of cyclohexanone and phenol are given by
Schmidlin and Lang, 1910.
CYTISINE (Ulexine) CUH16N2O (m. pt. I5i°-I5i.5°).
SOLUBILITY IN SEVERAL SOLVENTS AT 15°.
(Van de Moer, 1891.)
Q0iv<,nf Gms. CuHiRN2O QniWnt Gms- CuHwNjO per
bolvent. per ipo Gms. Sat. Sol. Solvent. 100 Gms. Sat. Sol.
Water soluble in all proportions Benzine 1.26
Alcohol " " " Petroleum Ether insol.
Chloroform " " Amyl Alcohol 0.303
Ether (d 0.725) 0.302 Carbon Disulfide insol.
Ether, abs. insol. Ethyl Acetate very soluble
28l
DEXTRIN
DEXTRIN CuH»Qio.
SOLUBILITY IN WATER. (Lewis, 1914.)
" In the case of dextrin, however, no matter how small an amount of water be
employed, under no condition does the concentration of the solution remain con-
stant, while on the other hand the addition of further solvent, never fails to
dissolve additional dextrin, although the use of no amount of water, however
large, will dissolve the whole of the sample."
100 gms. pyridine dissolve 65.44 gms. dextrin at 20-25°.
100 gms. aq. 50% pyridine dissolve 102 gms. dextrin at 20-25°.
(Dehn, 1917.)
DIACETYL TARTARIC ETHER (m. pt. 104°) DIACETYL RACEMIC
ETHER (m. pt. 84°).
Freezing-point lowering data for each of these compounds in ethylene bromide
and in p xylene are given by Bruni and Finzi, 1905.
DIBENZYL C6H5.CH2.CH2.C6H5.
Freezing-point lowering data for mixtures of dibenzyl and stilbene are given by
Garelli and Calzolari, 1899.
DIDYMIUM Ammonium NITRATE Di(NO3)3.2NH4NO3.
100 gms. H2O dissolve 292 gms. of the salt at 15°.
(Holmberg, 1907.)
DIDYMIUM SULFATE Di2(SO4)3.
SOLUBILITY IN WATER.
Gms.
(Marignac, 1853.)
t°.
per 100
Solid Phase.
Gms. H2O.
12
43.1
Di2(S04)3
18
25.8
tt
25
20. 6
tt
38
13
t(
50
ii
tt
19
40
So
100
per 100
Gms. H2O.
II.7
8.8
6-5
1.8 •
Solid Phase.
Di2(SO4)3.6H2O
Di2(SO4)3.8H2O
DIDYMIUM POTASSIUM SULFATE K2SO4.Di2(SO4)3.2H2O.
100 gms. H2O dissolve 1.6 grams of the double salt at 18°.
DIDYMIUM SULFONATES.
SOLUBILITY IN WATER.
Salt.
Didymium Benzene Sulfonate
' m Nitro Benzene Sulfonate
m Chloro
m Bromo " "
Chloro Nitro "
a Naphthalene Sulfonate Di(Ci0H7SO3)3.6H2O
1.5 Nitro " " Di(CioH6(N02)SO3)3.6H2O
1.6 "
1.7 " "
(Holmberg, 1907.)
Formula. t°.
Di(C6H5SO3)3.9H2O 15
Di(C6H4(NO2)SO3)3.6H2O 15
Di(C6H4ClS03)3.9H2O 15
Di(C6H4BrSO3)3.9H2O 15
Di(C6H4Cl(N02)S03*)3.i6H2O 15
IS
15
Di(CioH6(N02)S03)3.9H2O 15
Di(Ci0H6(NO2)SO3)3.9H2O 15
(Marignac.)
Gms.
Anhydrous
Salt per 100
Gms. H20.
S3-I
47-8
12.7
14-3
0.52
0.18
* (SO3:NO2:C1 - 1.3.6.)
DIETHYLAMINE see ETHYLAMINE, page 294.
DIONINE (Ethyl Morphine) Ci9H23NO3.
100 cc. H2O dissolve 0.2613 gm. Ci9H23NO3 at 20^.
loo cc. oil of sesame dissolve 0.5144 gm.
at 20°.
(Zalai, 1910.)
DIPHENYL 282
DIPHENYL CeHs-CeHfi.
100 grams absolute methyl alcohol dissolve 6.57 grams at 19.5°.
100 grams abs. ethyl alcohol dissolve 9.98 grams at 19.5°. (de Bruyn, 1892.)
Freezing-point data (Solubility, see footnote, p. i) are given for mixtures of
diphenyl + naphthalene by Washburn and Read (1915) and by Vignon (1891).
Results for diphenyl -f- phenanthrene and for diphenyl + triphenylmethane are
given by Vignon (1891).
DIPHENYLAMINE (C6H6)2NH.
RECIPROCAL SOLUBILITY OF DIPHENYLAMINE AND WATER, BY SYNTHETIC
I [METHOD.
(Campetti and del Grosso, 1913.) '
Cms. (C6H5)2 NH Cms. (C6H5)2NH Cms. (C6H5)2NH
t°. per 100 Gms. t°. per ipo Gms. t°. per ipo Gms.
Mixture. Mixture. Mixture.
231 1.48 305crit. t. 47.5 239 88.28
264 3.49 304 62.52 229 90.23
275 5.62 299 73.07 210 92.93
297 16.50 289 82.08 152 97-19
303 45.16 249 86.73
Similar data for the systems diphenylamine + ether and diphenylamine -f-
isopentane are given by Campetti, 1917.
SOLUBILITY OF DIPHENYLAMINE IN SEVERAL SOLVENTS.
Solvent. f. pe^gMLt. Authority.
Water 20-25 0.03 (Dehn, 1917.)
Methyl AlCOhol 14.5 45 . 2 (Timofeiew, 1894.)
" " 19-5 57-5 (de Bruyn, 1892.)
Ethyl Alcohol 14 . 5 39.4 (Timofeiew, 1894-)
" " 19.5 56 (de Bruyn, 1892.)
Propyl Alcohol 14.5 29.4 (Timofeiew, 1894.)
Pyridine 20-25 302 (Dehn, 1917.)
Aq. 50% Pyridine 20-25 two layers formed
SOLUBILITY OF DIPHENYLAMINE AND ALSO OF TRIPHENYLAMINE IN CARBON
DlSULFIDE. (Arctowski, 1895.)
NH(C6H^)2 in CS, N(C6H5)3 in CS,.
t°.
Gms. per 100
Gms. Solution.
t°.
Gms. per 100
Gms. Solution.
-88J
0.87
-83
I.9I
-117
0-37
-91
1.56
— 102
1.24
— II3|
0.98
SOLUBILITY OF DIPHENYLAMINE IN HEXANE AND IN CARBON DISULFIDE.
(Etard, 1894.)
Gms. NH(C«HE)j Gms. NH(CfiHR)2
$». per IPO Gms. Sol, in; t°t per 100 Gms. Sol, in:
Hexane. CS^T* Hexane. CS2. '
-60 ... 1.3 o 2.6 33.7
— 50 ... 2.2 +10 3.8 46.8
— 40 ... 3.8 20 6.7 60.9
-30 0.5 7.2 30 13.8 76
— 20 0.8 12.5 40 47
— io 1.4 21.6 50 94
283
DIPHENYLAMINE
FREEZING-POINT DATA FOR MIXTURES OF DIPHENYLAMINE AND OTHER
COMPOUNDS.
Diphenylamine
Diphenylmethylamine
+ Acetyldiphenylamine
4- Ethylene Bromide
-j- Naphthalene
+ a Naphthylamine
+ Nitronaphthalene
+ a and /3 Naphthol
-j- Paraffin
+ Phenanthrene
+ Phenol
-j- Resorcinol
-j- p Nitrotoluene
-{-2.4 Dinitrotoluene
-j- a Trinitrotoluene
-j- p Toluidine
+ Urethan
Phenol
(Boeseken, 1912.)
(Dahms, 1895.)
(Roloff, 1895; Vignon, 1891.)
(Vignon, 1891.)
(Battelli and Martinetti, 1885.)
'Vignon, 1891.)
(Palazzo and Battelli, 1883.)
(Narbutt, 1905.)
(Philip, 1903.)
(Vignon, 1891.)
(Giua, 1915.)
+ o Chlorophenol
Hexanitrodiphenylamine + a Trinitrotoluene
DIPHENYLAMINE BLUE.
SOLUBILITY IN SEVERAL SOLVENTS AT 23°.
(Vignon, 1891.)
(Pushin and Grebenschikov, 1913.)
(Bramley, 1916.)
(Giua, 1915.)
Solvent.
Methyl Alcohol
Ethyl
Amyl
(Szathmary de Szachinar, 1910.)
Gms. Diphenylamine Blue
per 100 Gms. Sat. Sol.
0.385
0.230
o . 049
Acetone
Aniline
Diphenylamine Blue
per 100 Gms. Sat. Sol.
°-i77
°-395
DIPHENYL SULFIDE (C6H5)2S, etc.
Freezing-point lowering data for mixtures of (CeHs^S + (C6H5)2Se,
(C6H6)2Te, (C6H6)2S + (C6H6)2O, (QH.),Se+(G,H.),Tef are given by Pascal (1912).
DYES.
Data for the distribution of 12 dyes between water and isobutyl alcohol at 25°,
are given by Reinders and Lely, Jr. (1912).
DYSPROSIUM OXALATE Dy2(C2O4)3.ioH2O.
100 cc. aq. 20% methylamine oxalate dissolve 0.276 gm. Dy^QjOOs- | (Grant and
" ethylamine " " 1.787 " \ James,
triethylamine " " 1.432 ) Wl)
EDESTIN and Edestin Salts.
SOLUBILITY IN AQ. SALT SOLUTIONS AT 25°.
(Osborne and Harris, 1905.)
The determinations were made by shaking an excess of the air-dry preparation
with 20 cc. of the salt solution, allowing the globulin to settle and determining
nitrogen in 10 cc. of the clear supernatant solution. The edestin or edestin salt
was calculated from the N. The results are given in the form of curves. The
following figures were read from the curve for the solubility of neutral edestin in
aq. NaCl.
Gms. NaCl per 20 cc. Solvent — » 0.468 0.585 0.702 0.818 0.935
Gm. Edestin per 20 cc. Sat. Sol. —> 0.25 0.55 0.92 1.25 1.45
Curves are also given for the solubility of edestin in aqueous solutions of many
other salts and of the solubility of edestin chloride, bichloride and sulfate in aq.
sodium chloride solutions.
100 gms. pyridine dissolve 0.07 gm. edestin at 20-25°. (Dehn, 1917.)
ioo gms. aq. 50% pyridine dissolve 9.05 gm. edestin at 20-25°.
ELATERIN 284
ELATERIN
ibo cc. 90% alcohol dissolve 0.09 gm. elaterin at 15-20. (Squire and Caines, 1905.)
100 cc. chloroform dissolve 4 gms. elaterin at 15-20. " "
EMETINE and Salts.
SOLUBILITY IN WATER.
(Carr and Pyman, 1914.)
c I* •p^rrv.nio *° Gms. Hydrated Salt
Salt- Formula. t. per I00 cc. Sat. Sol.
Emetine Hydrochloride C29H4oO4N2.2HC1.7H20 18 13 . i
" Hydrobromide C29H4oO4N2.2HBr.4H2O 17-18 1.9
" Nitrate C29H4oO4N2.2HNO3.3H2O 17-18 3.7
" Sulfate C29H4oO4N2.H2S04.7H2O 17-18 more than 100
ERBIUM OXALATE Er2(C2O4)3.i4H2O.
SOLUBILITY IN AQ. SULFURIC ACID AT 25°.
(Wirth, 1912.)
Solid Phase.
Er2(C204)3.i4H20
Normality of
Aq. H2SO4.
Gms. per 100 Gms. Sat. Sol.
' Er203-
Er2(QA)3.
2.l6
0.329
0.5144
3-n
0-493
0.7708
4-32
0.7036
1. 10
6.I7S
I .IO
1.72
ERBIUM Dimethyl PHOSPHATE Er2[(CH3)2PO4]6.
IOO gms. H2O dissolve 1.78 gm. Er2[(CH3)2PO4]6 at 25°. (Morgan and James, 1914.)
ERBIUM SULFATE Er2(SO4)3.8H2O.
SOLUBILITY IN WATER AND Aq.^H2S04 AT 25°.
(Wirth, 1912.)
[Gms. per ioo Gms.
Solid Phase.
Normality
of H2S04.
Gms. per
Sat.
ioo Gms.
Sol. Solid Phase
Normality
• of H2SO4.
[Gms. per
Sat.
ioo Gms.
Sol.
Er203.
Er.CSO,);,.
' Er203.
Er2(S04)3:
Water alone 7
•339
II
.94 ErzCSO^.SHzO 2
.16
3
.98
6.
473
O
.1
7
•389
12
.02 "
6
•175
0
•9352
i ,
52i
0
•505
6
.249
10
. 164
12
.6
0
.0852
0
,1386
I
.1
5
.256
8
•549
ERBIUM Bromonitrobenzene SULFONATE Er(C6H3Br.NO2.SO3, 1.4.2)3. 12H2O.
ioo gms. sat. solution in water contain 6.056 gms. anhydrous salt at 25°.
(Katz and James, 1913.)
ERUCIC ACID C8H17CH:CH(CH2)nCOOH.
SOLUBILITY IN ALCOHOLS.
(Timofeiew, 1894.)
Gms. Erucic Gms. Erucic
Alcohol. t°. Acid per ioo Alcohol. t°. Acid per ioo
Gms. Sat. Sol. Gms. Sat. Sol.
Methyl Alcohol — 2 2.25 Ethyl Alcohol '+21.4 63.4
+ 18 60.4 Propyl Alcohol - 2 10.2
21.4 62 " " +18 60.5
Ethyl Alcohol - 2 8.24 21.4 63
ERYTHRITOL (CH2OH.CHOH)2.
ioo gms. H2O dissolve 61.5 gms. erythritol at 20-25°. (Dehn« *9i7)
ioo gms. aq.^0% pyridine dissolve 8.47 gms. erythritol at 20-25°.
ioo gms. pyridine dissolve 2.50 + gms. erythritol at 20-25. (Dehn.Jigi?; Holty, 1905.)
285
ETHANE
uinr, ^2n6. SOLUBILITY IN WATER.
(Winkler, 1901.)
t°.
/9.
/S'.
3.
t°.
0.
/?'.
j.
O
0
.0987
o
.0982
0
.0132
40
0
.0292
o 0271
0.0037
5
0
.0803
0
.0796
0
.0107
50
o
.0246
0.0216
0.0029
10
0
.0656
0
.0648
0
.0087
60
0
.0218
0.0175
0.0024
15
0
•0550
0
.0541
0
.0073
70
0
.0195
0.0135
0.0018
20
0
.0472
0
.0462
o
.0062
80
o
.0183
0.0097
0.0013
25
0
.0410
0
.0398
0
.0054
90
0
.0176
0.0054
0.0007
30
0
.0362
o
•0347
0
.0049
100
o
.0172
o.oooo
o.oooo
/? = Absorption coefficient, i.e., the volume of gas (reduced to o°
and 760 mm.) absorbed by i volume of the liquid when the pressure
of the gas itself without the tension of the liquid amounts to 760 mm.
ft' = Solubility, i.e., the volume of gas (reduced to o° and 760 mm.)
which is absorbed by one volume of the liquid when the barometer
indicates 760 mm. pressure.
q = the weight of gas in grams which is taken up by 100 grams of
the pure solvent at the indicated temperature and a total pressure
(that is, the partial pressure of the gas plus the vapor pressure of the
liquid at the absorption temperature) of 760 mm.
Freezing-point data for mixtures of ethane and hydrochloric acid are given by
Baume and Georgitses, 1912, 1914.
SOLUBILITY OF ETHANE IN SEVERAL ALCOHOLS AND OTHER SOLVENTS.
(McDaniel, 1911.)
Solvent.
Methyl Alcohol (99%) 22.1
" " 30.2
40
49.8
Ethyl Alcohol (99.8%) 22,2
« «
(I U
Isopropyl Alcohol
Abs. coef. A = vol. of ethane absorbed by unit volume of solvent at the temp, stated.
For definition of Bunsen Coef. B, see /3 above, and also carbon dioxide, p. 227.
Additional data for the solubility of ethane in amyl alcohol are given by (Friedel
and Gorgeu, 1908).
ETHYL ACETATE CH3COOC2H5.
SOLUBILITY OF ETHYL ACETATE IN WATER AND VICE VERSA.
(Merriman, 1913, see also Seidell,1 1910.)
Results for Ethyl Acetate in Water. Results for Water in Ethyl Acetate.
Gms. H2O per 100
t°.
Abs.
Coef. A.
" Bunsen c/o™,,* *°
Coef. B. Solvent. t .
Abs.
Coef. A.
Bunsen
Coef. B.
22.1
0.4436
0.4102 Amyl Alcohol 22
0.4532
0.4196
30.2
0.4278
0.3883 " 30.1
0.4444
0.4002
40
0.3938
0.3436 Benzene 22.1
0.4954
0.4600
49.8
0.2695
0.2278
35
0.4484
0.3976
22.2
0.4628
0.4282
40.1
0.4198
0.3661
30-r
0.4503
0.4051
49.9
0-3645
0.3081
40
0.4323
0.3771 Tol
ene 25
0.4852
0.4450
21.5
0.4620
0.4275
3°
0.4778
0.4300
29.9
0.4532
0.4081
40.1
0.4675
0.4080
40
0.4400
0.3837
50.2
0-4545
0.4013
60.3
0.4244
0.3478
60
0.4502
0.3690
t°.
d£ of Sat. Sol.
Gms. CH3COOC2H5
per 100 Gms. H2O.|
0
5
* 1. 0034
1.0022
II. 21
10.38
10
I . OOOQ
9.67
15
20
25
0.9995
0.9979
0.9962
9-°5
8-53
8.08
30
0.9943
7.71
40
0.9901
7.10
t°.
d^ of Sat. S<
o
10
0.9280
0.9164
20
0.9054
25
3°
40
O.9OO2
0.8953
0.8863
50
60
. . .
2.34
2.68
3-07
3-30
3-52
4.08
4.67
5-29
ETHYL ACETATE
286
SOLUBILITY IN WATER AND IN AQUEOUS SALT SOLUTIONS AT 28°,
(Euler — Z. physik. Chem. 31, 365, '99; 49, 306, '04.)
Cone, of Salt
Solution.
CHgCOOCjiHs
per Liter.
Solvent. * -. /
Cone, of Salt
Solution.
CH3COOC2H»
per Liter.
^olvent.
Nor- Gms per
mality. Liter.
Gram
Mols.
Grams.
Nor- Gms. per Gram
nudity. Liter. Mols.
Grams.
Water
0
O
0.
825
75.02
NaCl(at 18°)
i
14.62
0.76
67.0
KNOa
i
5°
•59
O.
77
67.81
« «
i
29-25
0.67
59-o
M
I
101
.19
0.
72
63.40
« «
i
58.5
°-5I
45-o
It
2
202
.38
O.
625
55-04
Na2S04
i
71.08
0.465
40.96
KC1
i
18
•4
0.
747
65-79
" (at 18°)
i
35-54
0.61
54-0
«
i
36
.8
0.
685
65-33
(( (t
i
71.08
0.42
37-o
M
I
73
.6
O.
575
50.64
MgS04
1
16.30
o-733
64.55
« .
2
147
.2
0.
41
36. ii
a
i
32.6
0-655
57.68
Nad
\
14
.62
0.
745
65.61
(i
i
65.21
0-505
44-47
M
i
29
•25
0.
677
59.62
ZnSO4
1
20.18
0-733
64.55
«
I
58
•5
0.
545
47-99
«
i
40.36
0-653
57-50
M
2
117
.0
O.
3J5
27.74
u
i
80.73
0.500
44-03
Additional data for the influence of salts upon the solubility of ethyl acetate in
water are given by Lundin, 1913.
SOLUBILITY OF ETHYL ACETATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
cc. CH3COOC2H5 Gms. CH3COOC2H,
per TOO Gms.
Solvent.
8.6
10.9
13-3
19.6
37-o
66.7
00
SOLUBILITY OF ETHYL ACETATE IN AQUEOUS ETHYL ALCOHOL, METHYL
ALCOHOL, AND ACETONE MIXTURES AT 20°.
(Bancroft — Phys. Rev. 3, 122, 131, '95-' 96.)
In Ethyl Alcohol. In Methyl Alcohol. In Acetone.
Per i cc. C2H6OH.
Wt. «
in!
70 C2H5OH
Solvent.
d& of Sat.
Sol.
cc. CH3COO(
per 100 cc
Solvent.
0
o-999
10
5
0-993
10-5
10
0.986
12
15
0-974
15
20
0.960
27
25
0-945
44
30
0.931
70
35
0.918
125
40
CO
cc-HaO* ,
:H3COOC2H6.t
10
0.25
8
0.27
4
0-35
2
1.02
1. 06
2.50
0.65
5-0
0-54
7.0
0.44
10. 0
Per i
cc. CH3OH.
Per i
cc. (CH3)2CO.
cc. H2O.
CHaCObc-zHB.
cc. H2O.
CH3COOC2H8.
10
1. 08
10
1. 01
3
0.68
5
O.6o
*•$
1.69
2
o-43
1.29
2.50
I .5
0.47
1.0
4-9
I .O
0.63
0.98
7-o
0.8
o-74
I -O
8.0
0.51
1. 00
1.03
10. 0
0.25
2.00
0.29
5.00
1 acetate. t Saturated with water.
Data for the distribution of ethyl acetate between petroleum and water, ben-
zene and water, and benzene and a large number of aqueous solutions, at various
temperatures, are given by Philip and Bramley, 1915.
287
ETHYL ALCOHOL
RECIPROCAL SOLUBILITY OF ETHYL ALCOHOL AND WATER AT Low TEM-
PERATURES, DETERMINED BY THE FREEZING-POINT METHOD.
(Pictet and Altschul, 1895; Pickering, 1893.)
Cms.
t°. of
Freezing.
Sp. Gr. C2HBOH per Solid
Sat. Sol. 100 Gms. Phase.
Sat. Sol.
— I
0.9962
2.5 Ice
— 2
0.9916
4.8 «
- 3
0.9870
6.8 "
- 5
0.9824
11.3
- 6.1
0.9793
13-8 "
- 8.7
0.9747
17.5 "
- 9.4
0.9732
18.8
— 10.6
0.9712
20.3
— 12.2
o . 9689
22.1
-14
0.9662
24 . 2
-16
0.9627
26.7 ••
— 18.9
0.9578
29.9
t°. of Sp. Gr.
Freezing. Sat. Sol.
Gms.
QHjOHper Solid .
100 Gms. Phase.
Sat. Sol
-23.6 o
.9512
33-8
Ice
—28.7 o
.9417
39
H
- 33-9 o
.9270
46.3
"
— 41 o
.9047
56-1
"
- 50
68
"
- 60
. . .
75
H
- 70
. . .
80
«
- 80
. . .
83-5
"
— 100
. . .
89-5
"
— uSEutec.
. . .
93-5
" +C2H6OH
"~II5
96
QH6OH
— 110.5
. . .
100
"
The result for the eutectic and for the f.-pt. of C2H5OH are by Puschin and
Glagoleva, 1914, 1915; the other data for concentrations of C2HsOH above 70%
were obtained by exterpolation. Additional data for the freezing-point lowering
are given by Rozsa (1911).
Freezing-point lowering data for mixtures of ethyl alcohol and hydrochloric
acid are given by Maass and Mclntosh, 1913.
The distribution coefficient of ethyl alcohol between amylalcohol and water
was found by Fontein (1910) to be 1.13 at 15.5° and 1.21 at 28°.
MISCIBILITY OF ETHYL ALCOHOL WITH MIXTURES OF:
Benzaldehyde and Water at o°.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Benzene and Water at 15°.
(Bonner, 1910.) (See also, p. 125.)
Composition of Homogeneous Mixtures.
Gms.
Gms.
Gms.
Sp.
Gr. of
Gms.
Gms.
Gms.
Sp. Gr. of
QH5CHO.
H20.
C2H5OH.
Mixture. C6H6.
H20.
C2H5OH.
Mixture.
0-957
0.043
0
• 159
I
.02
O
.987
o
.013
0.170
0.86
0.898
O. IO2
O
.283
I
.OI
0
•937
0
.063
0.356
0.87
O.SOO
0.200
0
.420
0
•99
*0
.900
0.
100
0.500
0.86
0.700
0.300
O
• 550
O
.98
o
.800
o
.200
0.860
0.86
^0.598
O.4O2
O
.601
0
•97
0
.700
o
,300
0.910
0.88
0.430
0
.610
0
.600
o,
.400
1.07
0.87
0.496
0.504
o
•643
o
.96
o
.500
o
.500
1.18
0.87
0-394
0.606
o
.681
0
•95
o
.400
o
.600
I .22
0.88
0.298
0.702
0
.701
0
•95
0.300
o
,700
I. 21
0.89
0.200
0.800
0
.670
o
•95
o
.201
o,
799
I-I3
0.89
O.IOO
O.9OO
o
.610
0
.96
o
.100
o
.900
0.97
0.92
0.031
0.969
0
.461
o
•97
0
.020
o
.980
o-59
0.94
NOTE. — The determinations were made by gradually adding ethyl alcohol to
the mixtures of the given amounts of water and the other constituent until a
homogeneous solution was obtained. The results give the binodal curve for the
system. The author also determined "tie lines" showing the compositions of
various pairs of liquids which may exist in equilibrium. As the two layers
approach each other in composition, the tie line is gradually shortened and finally
reduced to a point, designated as the "plait point" of the binodal curve. This
point is indicated by a * in the above tables. The mixtures above and below the
* correspond, according to their Sp. Gr., to the upper and lower layers of the
system. See also, last table p. 289.
The distribution coefficient of ethyl alcohol between benzene and water at 25°
was found by Morgan and Benson (1907) to be 1.16. Additional data for this
system are also given by Bubanovic, 1913 and by Taylor (1897).
ETHYL ALCOHOL
288
'MISCIBILITY OF ETHYL ALCOHOL (see Note, p. 287) WITH MIXTURES OF:
Bromobenzene and Water at o°. Nitrobenzene and Water at 15°.
(Bonner, 1910.) (Bonner, 1910.)
Composition of Homogeneous Mixtures. Composition of Homogeneous Mixtures.
Cms. Cms. Cms. Sp. Gr.
Gms. Gms. Gms. Sp. Gr.
QH5Br. H2O. C2H5OH. Sat. Sol.
C6H8NO2. H2O. C2H5OH. Sat. Sol.
0.99 o.oio 0.115 I-34
0.965 0.035 0.248 I. 08
*o.96 0.040 0.32
*o.9i 0.09 0.49 ...
0.90 o.io 0.65 1.07
0.90 o.io 0.53 i. 02
0.80 0.20 I 0.96
0.80 0.20 0.86 0.97
0.70 0.30 I.I9 0.96
0.70 0.30 1.09 0.94
o . 60 o . 40 i . 30 o . 98
0.594 0.406 1.238 0.93
0.50 0.50 1.39 0.95
0.50 0.50 I.3I 0.92
0.40 0.60 1.43 0.91
0.40 0.60 1.34 0.92
0.30 0.70 1.43 0.92
0.30 0.70 1.30 0.91
O.2O O.8O 1.36 0.93
0.194 0.8o6 I. 212 0.92
o.io 0.90 1.16 0.93
o.io 0.90 0.98 0.93
0.024 0.976 0.803 °-92
0.02 0.98 0.601 0.95
MISCIBILITY OF ETHYL ALCOHOL (see
Note, p. 287) AT o° WITH MIXTURES OF:
Benzyl Acetate and Water. (Bonner, 1910.)
Benzyl Alcohol and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Cms. CH3.- Cms. Cms. Sp. Gr.
Gms. Gms. ' Gms. Sp. Gr.
CO2.CH2.QH5. H2O. C2H5OH. Sat. Sol.
C6H5CH2OH. H2O. Q,H5OH. Sat. Sol.
0.977 0.023 0.120 1.05
0.90 o.io 0.13 1.03
0.901 0.099 o-a1? i-°3
0.80 0.20 0.26 I
O.8O O.2OO 0.46 0.99
0.70 0.30 0.35 0.98
0.70 0.300 0.58 0.97
0.60 0.40 0.39 0.98
*o.68 0.32 0.60
0.50 0.50 0.40 0.97
0.60 0.40 0.69 0.95
0.40 O.6O 0.41 0.97
0.50 0.50 0.78 0.94
*o.38 0.62 0.42
0.40 0.60 0.85 0.94
0.379 0.621 0.417 0.98
0.30 0.70 0.88 0.93
0.30 0.70 0.41 0.97
0.20 0.80 0.88 0.93
0.194 0.806 0.388 0.97
o.io 0.90 0.80 0.94
o.io 0.90 0.35 0.98
0.041 0.959 0.665 °-95
0.04 0.96 0.139 0.99
MISCIBILITY OF ETHYL ALCOHOL (see
Note, p. 287) AT o° WITH MIXTURES OF:
Benzylethyl Ether and Water.
(Bonner, 1910.)
Carbon Tetrachloride and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Cms. Cms. Cms. Sp. Gr.
Gms. Gms. Gms. Sp. Gr.
CeHsCHj.O.QHs. H2O. CjHjOH. Sat. Sol.
CCU. H2O. C2H5OH. Sat. Sol.
0.971 0.029 0.189 °-94
0.961 0.039 0.224 1.36
0.90 o.io 0.37 0.92
0.928 0.072 0.347 1.23
0.80 0.20 0.54 0.92
*o«92 0.08 0.39
0.70 0.30 0.67 0.91
0.90 o.io 0.45 i. 20
*o.67 0.33 0.71
O.8O O.2O 0.67 I .15
0.60 0.40 0.78 0.91
0.70 0.30 0.82 1.07
0.50 0.50 0.87 0.91
o . 60 o . 40 o . 94 i . 03
0.40 0.60 0.93 0.92
0.499 °-5O1 1.04 i
0.30 0.70 0.96 0.92
0.40 0.60 i °-97
0.198 0.802 0.952 ,0.92
0.25 0.75 1.105 °-9S
o.io 0.90 0.86 0.93
o.io 0.90 i 0.92
0.08 0.92 0.793 °-94
0.032 0.968 0.745 0.93
289 ETHYL ALCOHOL
DISTRIBUTION OF ETHYL ALCOHOL AT 25° (Bugarszky, 1910) BETWEEN:
Bromobenzene and Carbon Tetrachloride and Carbon Disulfide and
Water. Water. Water.
Cms. C2H5OH per Liter. Cms. C2H5QH per Liter. Cms. QHsOH per Liter.
C6H5Br Layer* H2O Layer'. 'CO, Layer. H2O Layer." 'CSj Layer. H2O Layer.
0.72 18.5 0.45 18.7 0.27 IQ.I
1-36 36-9 o-93 36-5 1-87 37-
2.68 68.2 2.55 68.1 10.23 69.3
MISCIBILITY OF ETHYL ALCOHOL (see Note p. 287) AT o° WITH MIXTURES OF:
Chloroform and Water. (Bonner, 1910.) Diethylketone and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures. Composition of Homogeneous Mixtures.
Cms.
Cms.
Cms.
Sp,
Gr.
Cms.
Cms.
Cms.
Sp. Gr.
CHC13.
H20.
C2H6OH.
Sat
.Sol.
i-
H20.
Sat. Sol.
0.907
O
•093
0.434
I.
19
0.
938 '
0
.062
0.136
0.85
0.90
0
.10
0-45
I .
18
0.
900
O
.10
O.I9
0.85
0.80
O
.20
0.60
I.
12
O.
895
O
• 105
0.201
0.86
0.70
0
•3°
0.68
I .
07
0.
800
0
.20
0.31
0.87
0-593
0
•407
0.726
I.
04
0.
781
O
.219
0.317
0.87
0.501
O
•499
0.729
I .
03
0.
702
0
.298
0.356
0.88
"0.420
0
•58
0.73
. .
.
0.
600
0
.400
0.392
0.89
0.404
O
•596
0-733
I .
01
O.
547
O
•453
O.4IO
0.90
0.300
O
.70
0.70
O.
99
0.
499
0
.501
0.4II
0.91
0.197
0
.803
0.672
0.
98
O.
458
O
•542
0.415
0.92
O.IOO
O
.90
0.61
O.
98
0.
407
0
•593
0.404
0.91
0.088
0
.912
0.608
0.
98
Additional data for the miscibility of alcohol with chloroform + water mixtures
are given by Miller and McPherson, 1908.
MISCIBILITY OF ETHYL ALCOHOL WITH MIXTURES ^OF ETHYL ETHER AND
WATER AT O°. (Corliss, 1914; Bonner, 1910; see also Kremann, igioa.)
Composition of the Lower Layer. Composition of Upper Layer.
Cms.
(C2H5)20.
0.10
Cms.
H20.
0.90
Cms.
C2HBOH.
0.163
Sp. Gr.
Sat. Sol.
0.970
Cms.
(C2H6)20.
Cms.
H20.
Cms.
Sp. Gr.
Sat. Sol.
0.957
0
•043
O.I5I
0-757
0.16
0.84
O,
297
O
•951
O
.902
0
.098
0.230
0.778
0.178
0.822
O,
.318
O
•945
O
•87
O
• 13
0.26
0.788
0.192
0.8o8
0,
332
0
.941
0
.85
O
• 15
0.275
0.794
0.204
0.796
O
•34
O
•937
O
.825
0
• 175
0.292
0.800
0.227
0-773
O,
352
0
•932
O
•79
O
.210
0.313
0.808
0.250
o-75
0,
36
0
.926
0
•759
O
•243
0.33
0.815
0.293
0.707
O,
37
O
.916
0
•70
0
•30
0-35
0.827
0-335
0.665
0,
375
0
.906
O
•645
O
•355
0.366
0.839
0.422
0.578
O,
385
O
.886
0
•562
O
•438
0.385
0.857
"0.49
0.51
0
•385
O
.874
0
•49
0
•51
0.385
0.874
The data for the binodal curve given by Corliss and by Bonner agree closely.
The Sp. Gr. determinations of Corliss were made on larger amounts of solution
and appear to be the more accurate. In addition, Corliss gives the specific gravi-
ties of each layer of a series of liquids in contact with each other, and from these
and the binodal curve, the above data for the composition of the several con jugate
layers have been calculated. Data are also given by Corliss for the distribution
of colloidal arsenious sulfide between the two layers of the system.
Data for the distribution of ethyl alcohol between ether and water and between
ether and molten CaCl2.6H2O are given by Morgan and Benson (1907).
ETHYL ALCOHOL
290
MISCIBILITY OF ETHYL ALCOHOL WITH MIXTURES OF ETHYL ETHER AND
WATER AT 25°. (Horiba, 1911-12.)
Composition of Lower Layer. Composition of Upper Layer.
Gms.
Gms.
(QH5)20.
H20.
Gms. QH5OH.
5-77
94-23
0
6-3
85-7
8
7.2
79-2
13-6
8
76
16
9-7
70.4
19.9
13-3
62.8
23-9
22.1
50.6
27-3
28.4
43-4
28.2
*3i-6
40
28.4 (Plait point;
Gms.
Gms.
Gms.
H20.
QH5O2H.
98/72'
1.28
0
94-5
2.2
3-3
88.5
3-7
7-8
84-4
4-9
10.7
75.1
8.4
I6.5
60.8
iS-5
23-7
43-8
28.1
28.1
35-8
35-6
28.6
31-6
40
28.4
The binodal curve was determined in the usual way (see Note, p. 287). A series
of conjugate liquids was then prepared and the Sp. Gr., refractive index and
viscosity of each layer determined. From specially prepared curves for variations
of physical constants with composition of mixture, the composition of the several
conjugate liquids was ascertained. The results thus obtained, are given in the
above table.
Data for the miscibility of ethyl alcohol with mixtures of water, ethyl ether and
sulfuric acid at o° and with mixtures of ethyl ether, water and ethylsulfuric
acid at o° are given by Kremann, 19103.
MISCIBILITY OF ETHYL ALCOHOL (see Note p. 287) AT o° WITH MIXTURES OF:
Ethyl Acetate and Water. (Bonner, 1910.) Ethyl Bromide and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms.
Grns.
Gms.
Sp. Gr.
CHjCOOQHs.
H20.
C2H5OH.
Sat. Sol.
0.92
0.080
0.100
0.91
0.90
O.IO
0.13
0.91
0.799
O.2OI
0.228
o-93
0.699
O.3OI
0.265
0.92
0.60
0.40
0.29
o-95
0.50
0.50
0.30
o-95
*o.48
0.52
0.30
0.40
O.6O
0.31
0.96
0.30
O.7O
0.31
0.96
0.197
0.803
0.282
o-97
0.102
0.898
0.143
o-99
Gms.
Gms.
Gms.
Sp. Gr.
C2HBBr.
H20.
C2H5OH.
Sat. Sol.
0.967
0.033
O.24O
1.23
0.90
O.IO
0-37
I-I5
*o.83
0.17
0.45
0.80
O.2O
0-51
1.09
0.70
0.30
0.64
1. 06
0.60
0.40
0-754
1.03
0.50
0.50
0.83
I
0.40
O.6O
0.89
o-99
0.30
0.70
0.89
o-97
O.IO
0.90
o-73
0-97
0.017
0.983
0.182
o-99
MISCIBILITY OF ETHYL ALCOHOL (see Note p. 287) AT o°, WITH MIXTURES OF:
Ethyl Buty rate and Water. (Bonner, 1910.) Ethyl Propionate and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms.
0.97
0.90
0.80
0.70
0.599
0.494
*o.46
0.40
0.297
0.193
O.JO
Gms.
H20.
0.030
o.io
0.20
0.30
0.401
0.506
0.54
0.60
0.703
0.807
0.90
Gms. ' Sp.Gr.
C2H5OH. Sat. Sol.
0.166 0.96
0.32
0.483
0.567
0.628
0.659
0.67
0.69
0.693
0.88
0.89
0.90
0.91
Gms. Gms.
CjHjCOOQNj. H2O.
0.977 0.023
0.90 o.io
0.80
0.695
0.60
Gms.
0-684
0.63
0.92
o-93
o-94
0.94
0.50
*o.46
0.398
0.30
0.201
o.io
0.20
°-3°5
0.40
0.50
0.54
0.602
0.70
0.799
0.90
0.138
0.27
0.38
°-453
0.49
0.52
0.53
0.532
0.55
°-5I7
0.46
Sp. Gr.
Sat. Sol.
0.90
0.90
0.90
o-92
0.91
0.92
0.93
0.94
°-95
0.96
291
ETHYL ALCOHOL
MISCIBILITY OF ETHYL ALCOHOL (see Note, p. 287) AT o° WITH MIXTURES OF ;
Ethylene Chloride and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Cms. Cms. Cms. Sp. Gr.
CH2C1.CH2C1. H2O. CjH.,OH. Sat. Sol.
O.pyi 0.029 0.191 I.I5
0.90 o.io 0.42 i. 08
*O . 88 O . 1 2 0 . 46 ...
0.792 0.208 0.670 i. oi
O.7O 0.30 O.8O 0.98
O.6O 0.40 0.93 0.96
0.50 0.50 0.99 0.95
0.40 0.60 i.oi 0.94
0.30 0.70 0.99 0.94
O.2O O.8O 0.95 0.94
O.O95 0.905 0.842 0.96
0.02 0.980 0.514 0-97
Ethylidene Chloride and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Cms. Cms. Cms. Sp. Gr.
CH3.CHCI2. H20. QHjOH. Sat. Sol.
0.985 0.015 0.226 i. 10
0.90 o.io 0.43 1.03
0.805 °-I95 0.586 i.oi
O.yO 0.30 0.69 0.98
*o.67 0.33 0.72
0.60 0.40 0.77 0.96
0.50 0.50 0.82 0.95
0.437 0-563 o-857 0.94
0.30 0.70 0.88 0.93
0.20 0.80 0.86 0.93
o.io 0.90 0.79 0.94
0.03 0.97 0.576 0.95
MISCIBILITY OF ETHYL ALCOHOL (see Note, p. 287) AT o° WITH MIXTURES OF:
Heptane and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Cms.
Heptane.*
Gms. Gms. Sp. Gr."|
H20. C,H5OH. Sat. Sol.
0.962 0.038 0.704 0.79
0.90 o.io 1.44 0.80
0.798 0.202 2.375 0.82
0.70 0.30 2.82 0.81
0.60 0.40 3.06 0.82
0.50 0.50 3.16 0.83
o . 40 o . 60 3 . 1 7 o . 84
0.30 0.70 3.10 0.85
0.196 0.804 2.96 0.87
0.093 0.907 2.305 0.88
Hexane and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Gms.
Hexane.
Sp. Gr.
Sat. Sol.
Gms. Gms.
H2O. C2H8OH.
0.97 0.03 0.59
0.90 o.io 1.30 0.77
0.80 0.20 2.04 0.79
0.70 0.30 2.45 0.81
0.60 0.40 2.73 0.82
0.50 0.50 2.93 0.83
o . 40 o . 60 3 . oo o . 83
0.20 0.80 2.75 0.85
o.io 0.90 2.23 0.86
0.014 0.986 1.056
Kahlbaum's Heptane and Hexane "aus Petroleum " were used.
MISCIBILITY OF ETHYL ALCOHOL (see Note, p. 287) AT o° WITH MIXTURES OF:
Isoamyl Alcohol and Water.
(Bonner, 1910.) ,
Composition of Homogeneous Mixtures.
Gms. (CH3)2- Gms. Gms. Sp. Gr.
CH(CH2)2OH. H20. C2H5OH. Sat. Sol.
0.903 0.097 0.116 0.84
0.90 O.IO O.I2 0.84
0.797 O.2O3 0.258 0.85
0.694 0.306 0.396 0.86
0.602 0.398 0.427 0.88
0.497 °-5°3 °-449 0.89
0.399 0.601 0.453 0.90
0.294 0.706 0.434 0.92
*o.27 0.73 0.43
0.196 0.804 0.411 0.94
o.io 0.900 0.369 0.96
Isobutyl Alcohol and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Gms. (CH,),- Gms.
CH.CH2OH. H20.
Gms.
Sp. Gr.
Sat. Sol.
0.70 0.30 0.13 0.87
0.589 0.4II 0.177 0.89
0.502 0.498 0.194 0.90
0.50 0.50 0.20 0.90
0.40 O.6O O.2O 0.92
0.387 0.613 0.204 0.92
*o.35 0.65 0.21
0.304 0.696 0.205 0.94
0.30 0.70 O.2I 0.94
O.2O O.8O O.2O °-95
0.132 0.868 0.189 0.96
ETHYL ALCOHOL
292
MISCIBILITY OF ETHYL ALCOHOL (see Note, p. 287) AT o° WITH MIXTURES OF:
Isoamyl Bromide and Water. (Bonner, '10.)
Composition of Homogeneous Mixtures.
Iso butyl Bromide and Water. (Bonner, '10.)
Composition of Homogeneous Mixtures.
Gms. Cms. Cms. Sp. Gr.
Gms. (CH3)r Gms. Gms. Sp. Gr.
CsHuBr. H2O. QH6OH. Sat. Sol.
CHCH2Br. H2O. CjH6OH. Sat. Sol.
0.975 0.025 0-251 i-io
0.976 0.024 0.200 1.18
*o . 96 o . 04 0.36
*o.93 0.07 0.42
0.90 o.io 0.68 i.oi
0.90 o.io 0.52 1.09
0.80 0.20 1.09 0.96
0.80 0.20 0.83 I.OI
0.70 0.30 1.37 0.94
0.70 0.30 .05 0.98
0.60 0.40 1.57 0.93
O.6O 0.40 .21 0.96
0.498 0.502 .676 0.91
0.501 0.499 -3° °-94
0.40 0.60 .75 0.91
0.40 0.60 .35 0.93
0.30 0.70 .75 0.91
0.30 0.70 .36 0.93
O.2O O.8O .71 0.91
O.2O O.8O .32 0.92
o.io 0.90 .46 0.92
o.io 0.90 .20 0.93
0.022 0.978 .027 0.93
0.047 0.953 0.937 0.94
MISCIBILITY OF ETHYL ALCOHOL (see
Note, p. 287) AT-O° WITH MIXTURES OF:
Isoamyl Ether and Water. (Bonner, '10.)
Mesitylene and Water. (Bonner, '10.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms. f(CH3)2.- Gms. Gms. Sp. Gr.
Gms. Gms. Gms. Sp. Gr.
CH.CH2CHd2O. H20. C2H5OH. Sat. Sol.
C6H3(CHa)3. HjO. CjHjOH. Sat. Sol.
0.958 0.042 0.368 0.81
*o.97 0.03 0.48
0.90 o.io 0.70 0.82
0.963 0.037 o-S1^ 0.86
*o . 89 o . 1 1 o . 74 ...
0.90 o.io 1.09 0.85
0.879 O.I2I 0.793 0-82
o . 80 o . 20 i . 66 o . 84
0.80 0.20 1.20 0.83
0.70 0.30 2.04 0.85
0.702 0.298 1.573 0.83
0.60 0.40 2.32 0.85
0.594 0.406 1.876 0.84
0.50 0.50 2.52 0.85
0.50 0.50 1.98 0.84
0.40 0.60 2.64 0.86
0.40 0.60 2.19 0.85
0.30 0.70 2.68 0.87
0.302 0.698 2.24 0.86
0.199 0.801 2.49 0.87
0.20 0.80 2.14 0.87
o.io 0.90 2.28 0.89
o.io 0.90 1.87 0.89
0.051 0.949 1.615 0.90
MISCIBILITY OF ETHYL ALCOHOL (see
Note, p. 287) AT o° WITH MIXTURES OF:
Methyl Aniline and Water. (Bonner, '10.)
Phenetol and Water. (Bonner, '10.)
1 ' Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms. Gms. Gms. Sp. Gr.
Gms. Gms. Gms. Sp. Gr.
CHjNHQHj. H20. QHsOH. Sat. Sol.
QHsOCzHs. H2O. C2H5OH. Sat. Sol.
0.959 0.041 0.218 0.96
0.992 0.18 0.157 0.96
0.90 o.io 0.37 0.95
*o.9o o.io 0.55 ...
0.795 0-205 0.555 0.93
0.897 0.103 0.554 0.93
0.70 0.30 0.68 0.93
0.798 0.202 0.916 0.90
*o.66 0.34 0.72
0.70 0.30 .l8 0.90
0.60 0.40 0.76 0.93
O.6O O.4O .39 0.89
0.50 0.50 0.84 0.93
0.495 °-5°5 •51^ 0-89
0.40 0.60 0.89 0.93
0.399 0.601 .560 0.89
0.30 0.70 0.91 0.93
0.30 0.70 .54 0.90
0.20 0.80 0.87 0.94
0.198 0.802 .449 0.91
0.098 0.902 0.734 0.95
O.IO 0.90 .21 0.92
0.041 0.959 0-581 0.96
0.082 0.918 .156 0.93
293
ETHYL ALCOHOL
MISCIBILITY OF ETHYL ALCOHOL (see
Pinene and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Note p. 287) AT o° WITH MIXTURES OF:
Propyl Bromide and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Cms. Cms. Cms. Sp. Gr. '
Gms. Gms. Gms. Sp. Gr.
C,0H,,. H20. QH6OH. Sat. Sol.
CH3.CH2.CH2Br. H2O. QH6OH. Sat. SoL
0.99 o.oio 0.268 0.87
0.975 0.025 0.190 1.26
*o.985 0.015 0.47
*o.92 0.08 0.42
0.897 0.103 1.595 0.85
0.90 O.IO 0.50 1. 12
0.795 0.205 2.268 0.84
O.8O O.2O 0.72 I. 06
0.70 0.30 2.67 0.84
0.70 0.30 0.88 1.02
0.60 0.40 2.94 0.85
0.60 0.40 i.oi 0.99
0.493 °-5°7 3-!35 0-85
0.50 0.50 i.io 0.98
0.393 0.607 3.126 0.86
0.40 0.60 1.15 0.96
0.293 0.707 3.038 0.86
0.30 0.70 1.14 0.95
0.194 0.806 2.799 0-87
O.2O4 0.796 I. 12 0.94
0.094 0.906 2.331 0.89
0.096 0.904 1.02 0.94
0.035 0.965 1.639 0-91
0.027 0.973 0.687 0.95
MISCIBILITY OF ETHYL ALCOHOL (see
Note p. 287) AT b° WITH MIXTURES OF:
Toluene and Water. (Bonner, 1910.)
o Toluidine and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms. Gms. Gms. Sp. Gr.
Gms. Gms. Gms. Sp. Gr.
C6H5CH3. H20. QHsOH. Sat. Sol.
CH3.C6H4.NH2. H2O. QHsOH. Sat. Sol.
0.948 0.052 0.388 0.87
0.954 0.046 0.025 I-°I
0.90 o.io 0.61 0.86
0.90 O.IO O.2I 0.93
0.80 0.20 0.95 0.86
0.80 0.20 0.32 0.97
0.70 0.30 .21 0.86
0.70 0.30 0.41 0.96
0.60 0.40 .41 0.86
0.60 O.40 0.455 O-Q^
0.50 0.50 .53 0.87
0.50 0.50 0.48 0.96
0.40 0.60 .59 0.87
0.40 O.OO 0.50 0.96
0.30 0.70 .56 0.88
0.30 0.70 0.50 0.96
0.20 0.80 .44 0.89
0.20 0.80 0.49 0.96
o.io 0.90 .23 0.91
0.098 O.9O2 0.462 0.98
0.028 0.972 0.817 0.94
0.027 0-973 0.262
MISCIBILITY OF ETHYL ALCOHOL (see
Note p. 287) AT o° WITH MIXTURES OF:
Bromotoluene (b. pt. 182-3) and Water.
p Nitrotoluene and Water.
(Bonner, 1910.)
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms. Gms. Gms. Sp. Gr.
Gms. Gms. Gms. Sp. Gr,
BrC6H4.CH3. H2O. CjHsOH. Sat. Sol.
NO2.C6H4.CH3. H2O. QH6OH. Sat. Sof.
o . 98 o . 02 o . 33
0.978 0.022 0.253 I. 08
0.951 0.049 O.522 I.OQ
*o«95 0.05 0.50
0.90 o.io 0.87 i. 06
0.90 o.io 0.84 0.97
0.80 0.20 .28 0.97
O.8O O.2O 1.29 0.96
O.yO 0.30 .54 0.94
0.70 0.30 1.57 0.92
O.6O O.40 .71 0.93
0.00 0.40 1.73 0.91
O.5O O.50 .8l 0.92
0.506 0.494 1.782 0.91
O.4O O.6O .89 0.91
0.398 0.602 1.868 0.91
O.30 O.70 .89 0.90
0.294 0.706 1.816 0.91
O.20 0.80 .78 0.90
0.20 0.80 1.63 0.91
o.io 0.90 .533 0.91
o.io 0.90 1.30 0.92
0.033 0.967 1.307 O.Q2
0.056 0.944 1.105 0.93
ETHYL ALCOHOL
294
MISCIBILITY OF ETHYL ALCOHOL (see Note p. 287) AT o° WITH MIXTURES OF:
o Xylene and Water. (Bonnet, 1910.)
Composition of Homogeneous Mixtures.
m Xylene and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
'
Gms.
Gms.
Gms.
Sp. Gr.
Gms.
Gms. Gms.
Sp. Gr.
o C,H4(CH3),.
H20.
QH6OH.
Sat. Sol.
Hn C^g-tl^v^ji^g. H^O. C^HsOH.
Sat. Sol.
0.971
0.029
0-352
0.89
0.
967
0.
033 0.388
0.88
4
0.04
o-53
. . .
0.
90
O.
10 0.81
0.87
0.90
O.IO
0-93
0.87
o.
80
O.
20
-30
0.85
0.786
0.214
•32
0.87
0.
70
0.
30
.61
0.86
0.70
0.30
•53
0.87
0.
60
O.
40
•77
0.86
O.6O
0.40
.72
0.87
0.
50
0.
50
.90
0.87
0.50
0.50
.87
0.87
0.
40
0.
60
.98
0.87
0.40
0.60
.96
0.88
o.
30
o.
70
.01
0.88
0.30
0.70
•94
0.88
0.
20
0.
86
•87
0.89
O.2O
0.80
.81
0.89
0.
10
0.
9°
•53
0.90
O.O3I
0.969
.19
0.03
o.
023
o.
977
.168
O.O2
Additional data
for the system ethyl alcohol,
m xylene,
water at o°,
19°, 41°,
63
0 and 1 00° are given by Holt and
Bell, 1914.
p XYLENE AND WATER. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms.
Gms.
Gms.
Sp. Gr.
Gms.
Gms.
Gms.
Sp. Gr.
P C6H4(CHa)2. H20.
C2H5OH.
Sat
.Sol.
*C6H4(CH3)2. H20.
QH5OH.
Sat. Sol.
0.966
0.034
O.
.306
O,
84
0
•5°
O
•50
1.68
0.86
*0.92
0.08
0.
57
0
.40
O
.60
1.77
0.86
0.90
O.IO
0,
65
0,
•8S
0
.292
0
.702
1-743
0.87
0.80
0.20
I,
°5
o
•8S
O
• 193
o
.807
1.625
0.88
0.70
0.30
I,
•35
o
.85
0
.100
o
.90
i-39
0.89
0.60
T*t- -
0.40
ft*. . .
J (
A
0
•85
0
1 t 1
.015
_ _ 1 1 A
0
•985
0.863
0-93
The coefficient of distribution of ethyl alcohol between olive oil and water is
O.026 at 3° and 0.047 at 30°. (Meyer, 1901; 1909.)
100 gms. cottonseed oil (0.922 Sp. Gr.) dissolve 22.9 gms. ethyl alcohol at 25°.
100 gms. ethyl alcohol dissolve 11.75 gms. cottonseed oil at 2 5°. (Wroth and Reid, '16.)
DISTRIBUTION OF ETHYL ALCOHOL BETWEEN COTTONSEED OIL AND
WATER AT 25°. (Wroth and Reid, 1916.)
Gms. C2H5OH per 100 cc.
Oil Layer.
H20 Layer."
JXCLLiU*
o . 2083
6.147
29-5
0.2251
6.738
29.9
0.25I5
6-835
27.1
0.2783
6.876
24.7
°/3°1I7.,.
8.682
f , 1 1 t 1
28.7
Data for the reciprocal solubility of ethyl alcohol and turpentine are given by
Vezes and Mouline, 1904, 1905-06.
Data for the system ethyl alcohol, water, petroleum are given by Rodt (1916).
ETHYLAMINES C2H5.NH2, (C2H6)2NH, (C2H6)3N.
Freezing-point data (solubility, see footnote, p. i) for mixtures of ethylamine +
water, diethylamine + water, and triethylamine + water are given by Guthrie,
1884 and by Pickering, 1893.
The solubility of ethylamine and of diethylamine in water at 60°, calculated
from the vapor pressures determined by an aspiration method, are given by Doyer,
(1890) as follows:
A • Vapor Pressure in Ostwald Solubility Bunsen Absorption
mm. Hg. Ex. / (see p. 227.) Coef. (see p. 227.)
C2H5NH2 64.5 321 263
(C2H6)2NH 233 89 73
Data for the solubility of triethylamine in water at high pressures are given by
Kohnstamm and Timmermans, 1913.
295
ETHYL AMINES
SOLUBILITIES OF Di ETHYL
AMINE AND WATER.*
(Lattey — Phil. Mag. [6] 10, 398, '05.)
Gms. NH(C2H5)2
per 100 Gms.
0
Aqueous
Amine
'
Layer.
Layer.
155
21.7
59-O
150
23-6
55-5
148
24.8
53-5
146
26.3
51.0
145
28.0
49.0
144
31.0
45 -°
DISTRIBUTION OF TRI ETHYL AMINE
BETWEEN WATER AND AMYL
ALCOHOL AT 25°.
(Herz and Fischer — Ber. 37, 4751, '04.)
Cms. N(C2H5)3 • Millimols N(C2H6)»
per 100 cc. per 10 cc.
Aqueous
Layer.
Alcoholic
Layer.
Aqueous
Layer.
Alcoholic
Layer.
0.0885
0.1683
0.1866
0.2502
2.299
4-457
4.922
6.491
0-0875
0.1664
0.1846
0.2474
2.273
4-408
4.868
6.418
143.5 (crit- *•) 37-4
TriethylAMINE N(C2H5)3.
t°.
1 8. 6 (crit. temp.)
20
25
30
35
SOLUBILITY IN WATER.*
(Rothmund, 1898.)
Gms. NCCjH^s per 100 Gms. f0
Gms. N(C2H5)3 per 100 Gms.
Aq. Layer.
Amine Layer.
Aq. Layer.
Amine Layer
>•)
51-9
40
3^5
96.48
14.24
72
50
2.87
96.4
7-3°
95.l8
55
2-57
96.3
96.60
60
2.23
96.3
4.58
96.5
65
1.97
96.3
SOLUBILITY OF TRIETHYLAMINE IN WATER AND IN AQ. ETHYL ALCOHOL
AT DIFFERENT TEMPERATURES.*
(Meerburg, 1902.)
Water.
13-33% Alcohol. 28.98% Alcohol. 38.84% Alcohol. 60.16% Alcohol.
din. ^((^2x15)3
(jrHl. ^((^2X15) 3
Gm.N(C2Hfi)3 Gm.N(C2H5j3 Gm.N(C2H5)
t°. per 100 t°.
Gms. Sol. <
per zoo
jms. Sol.
t . per loo
Gms. Sol.
t . per loo t°. per loo
Gms. Sol. Gms. Sol.
69.2
I
•7
38.
3
8.2
54-
5
22
.8
73-4
31.2 76-77 71.2
30.8
5
.6
3i-
7
13-9
45
29
.8
65-4
33-3 74-75 75
23.1
8
5
28
21.6
33
4
51
.1
51.6
40.6 72-73 80
I8.7
25
.8
26.
4
30.6
3i
4
63
•7
42.1
50.6
I8.7
37
.2
24.
9
40-5
30
3
68
•5
40.9
54-7
19-5
.8
24.
2
49.8
28,
•5
82
.2
34-2
70.6
20.5
68
.6
24.
I ,
60.7
35
91
.8
33
77-5
20.5
84
24
69.7
34-7
88
20.5
89
•7
23-
5
76.6
40-5
91.3
21.2
92
•4
24
81.5
25.8
95
•5
24.
2
87.4
-
26.5
96
.1
25
92
NOTE. — Results for triethylamine, water and ethyl ether, and for triethyl-
amine, water and phenol are also given by Meerburg.
100 gms. abs. methyl alcohol dissolve 57.5 gms. NH(C6H5)2 at 19.5°.
100 gms. abs. ethyl alcohol dissolve 56 gms. NH(C6H5)2 at 19.5°.
(de Bruyn, 1892.)
* Determinations made by "Synthetic Method," see Note, p. 16.
Results
at 1 8°.
Results
at 25°.
Results at
32.35°.
Cms. Equiv.
per Liter
Aq. Layer.
Partition
Coef.
Gms. Equiv.
per Liter
Aq. Layer.
Partition
Coef.
Gms. Equiv.
per Liter
Aq. Layer.
Partition
Coef.
0.0756
26.09
O.II59
I9-I3
0.1287
14.76
0.0886
26.14
0.0999
19.11
0.2479
14.79
o . 0484
2.14
0.0483
i-59
0.1200
1.093
0.0503
2.14
O.O4l6
i-59
O.IIO4
1.095
0.0189
O.I3I
O.OIO4
0.099
0.0132
0.069
O.OI9I
O.I3I
O.OI3I
0.099
0.0133
0.069
ETHYLAMINES 296
DISTRIBUTION OF ETHYLAMINES BETWEEN WATER AND TOLUENE.
(Moore and Winmill, 1912.)
Amine.
(C2H5)NH2
a
(C2Hs)2NH
(C2H5)3N
Similar data for triethylamine at 25° and at other, temperatures are given by
Hantzsch and Sebaldt, 1899, and by Hantzsch and Vagt, 1901.
Data for ternary systems composed of triethylamine, water and each of the
following compounds: naphthalene, cane sugar, KC1, K2CO3, K2SO4 and KSCN,
are given by Timmermans (1907).
ETHYL, DiETHYL and TriETHYLAMINE HYDROCHLORIDES, etc. v
SOLUBILITY OF EACH IN WATER AND IN CHLOROFORM AT 25°.
* ' (Peddle and Turner, 1913.)
Solubility in Water. Solubility in CHC13.
Amine Salt. Formula. Gms. Amine Salt Gms. Amine Salt
per loo Gms. H2O. per 100 Gms. CHC13.
Ethylamine Hydrochloride C2H5.NH2.HC1 279.9 0.17
Diethylamine " (C2H5)2NH.HC1 231.7 29.45
Hydrobromide (C2H5)2NH.HBr 311.6 46 . 65
" Hydroiodide (C2H5)2NH.HI 377.2 71.56
Triethylamine Hydrochloride (C2H5)3N.HC1 137 17.37
Hydrobromide (CjjHs^N.HBr 150.6 23 . 44
Hydriodide (CjjHysN.HI 370 92.2
ETHYL BROMIDE C2H6Br.
SOLUBILITY IN ETHER. (Parmentier, 1892.)
t°. —13°. O. 12. 22.5. 32.
Gms. C2HsBr per ioo gms. Ether 632 561 462 302 253
SOLUBILITY OF ETHYL BROMIDE, ETC., IN WATER.
(Rex, 1906.)
Grams per 100 Grams H2O at:
Dissolved Substance. t * N
o . 10 . 20°. 30°.
Ethyl Bromide i . 067 o . 965 o . 914 o . 896
Ethyl Iodide 0.441 0.414 0.403 0.415
Ethylene Chloride 0.922 0.885 0.869 0.894
Ethylidene Chloride 0.656 0.595 °-55° 0.540
ETHYL BUTYRATE C3H7COOC2H5.
SOLUBILITY IN WATER AND IN AQUEOUS ETHYL ALCOHOL MIXTURES AT 20°.
100 g. H2O dissolve 0.5 g. ethyl butyrate at 22°. (Traube, 1884.)
100 cc. H2O dissolve 0.8 cc. ethyl butyrate at 20°. (Bancroft, 1895.)
100 cc. ethyl butyrate dissolve 0.4 — 0.5 cc. H2O at 20°.
Per 5 cc. (cc. H2O 10 6 4 2.96 2.10
Ethyl Alcohol j cc. C3H7COOC2H5 o . 34 o . 96 2 . 47 4 6
ETHYL CARBAMATE (Urethan) CO(OC2H5)NH2. See also p. 741.
SOLUBILITY IN SEVERAL SOLVENTS AT 25°. (U. s. P. vin.)
Solvent. Water. Alcohol. Ether. Chloroform. Glycerol.
Gms. CO(OC2H5)NH2 )
per 100 gms. solvent } I00+ l66 IO° 77 33
297
ETHYL ETHER (C2H6)2O.
RECIPROCAL SOLUBILITY OP ETHER
ETHYL ETHER
AND WATER.
(Klobbie— Z.physik.Chem. 24, 619, '97$ Schuncke — Ibid. 14,334. '94; St. ToUoczko — Ibid. 20, 407,
•96.)
Solubility of Ether in Water,
Lower Layer — Aqueous.
Gms.(C2H5)2O per 100 Cms.
Solubility of Water in Ether.
Upper Layer — Ethereal.
Gms. H2O per 100 Gms.
Water. Solution.
o 13-12 ii. 6
5 11.4 10.2
10 9.5 8.7
15 8.2 7.6
I
^ther. So
.01 ]
.06
.12 ]
.16
,».20 ]
lution.
• O
•05
.12 (2.6,
•*5
S.)
Jii
25 6-oS 5-7
30 54 5-1
*4o 4-7 4-5
*5° 4-3 4-i
*6o 3-8 3-7
*7o 3-3 3-2
*8o 2.9 2.8
.26
•33
•52
•73
•83
J.04 j
J.25 i
.26
•32
•50
•7
.8
J.O
} .2
* Indicates determinations made by Synthetic Method, for which see page 16,
ioo cc. H2O dissolve 8.11 cc. ether at 22°; vol. of solution, 107.145 cc., Sp.
Gr. 0.9853.
ioo cc. ether dissolve 2.93 cc. HzO at 22°; vol. of solution, 103.282 cc.; Sp..Gr.
0.7164. (Herz, 1898.)
More recent determinations of the solubility of ethyl ether in water, agreeing
closely with the above data, are given by Osaka, 1910.
Data for the temp.-pressure diagram of ether-water are given by Scheffer, 19123.
SOLUBILITY OF ETHER IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID.
(Schuncke — Z. physik. Chem. 14, 334, '94; in 38-52% HC1, Draper— Chem. News, 35, 87, '77.)
In
38.52 %HC1. In 31.61 %H
Cl. In 20 % HC1.
-6
o
+ 6
cc. Ether cc. Ether Gms. per i
per ioo cc. per ioo cc.
Solvent. Solvent. HC1-
181 149 0.4622
177.5 T42 0.4622
172.5 I3I-5 0.4622
Gram H2O. cc. Ether Gms. per i g. H2O.
(C2H5)2O. Solvent. HC1. (C^g)^.
.387 67.2 0.253 0-5637
.308 58.3 0.253 0-4863
.2075 51-1 o-253 0.4231
15
163 121.7(14°) 0.4622
•1075 40-5 0.253 0.3299
20
158 in .9 (20.8°) 0.4622
•0005 33.1 0.253 0.2688
26
135 104.2 0.4622
0.9360 27.5 0.253 0.2221
In i2.58%HCl.
In 3.65 %HC1.
to
cc. Ether per Gms. per i Gram H2O.
cc. Ether per Gms. per i Gram H2O.
•
ioo cc. Solvent. HC1. (C2H5)2O.
ioo cc. Solvent. HC1. (C2Hfi)2O.
-6
26.45 0.144 0.2106
19.23 0.0308 0.1454
o
22. 19 O-I44 0.1748
...
+6
19.18 0-144 0-1503
14.31 0.0308 0.1070
15
I5.6l 0.144 0-I2IO
11.83 0-0308 0.0868
20
13.76 0-144 0.1059
10.52 0-0308 0-0769
26
12.70 0.144 0.0970
9.24 0-0308 0-0673
The above data are recalculated and discussed by Juttner, 1901.
ETHYL ETHER
298
Data for the solubility of ethyl ether in carbon dioxide at high pressures are
given by Sander (1911-12). The determinations were made by using quite small
amounts of ether and observing the pressure at which a drop of liquid just
appeared or disappeared in a mixture of known weight per cent composition.
The results give the "gas curve" for constant temperature and when plotted in
connection with the " liquid curve" (see CO2, p. 233), give the complete pressure
— concentration diagram.
Freezing-point lowering data for mixtures of ethyl ether and hydrochloric acid
are given by Maass and Mclntosh (1913).
SOLUBILITY OF ETHER IN AQUEOUS SALT, ETC., SOLUTIONS AT 18°.
(Euler, 1904.)
Aq. Solu-
tion of:
Aq. Solu-
tion of:
vjms. per
Liter Added
Salt.
oms. (.L^tii
per 100 c
Solvent,
Water
0
7.8
KN03
lOI.ig
5-4
KC1
73-6
4-7
LiCl
42.48
5-2
NaCl
58-5
4-5
Mannite
H2S04
Gms. per
Liter Added
Gms. (CjHs^O
per 100 cc.
Salt.
Solvent.
59-54
3-7
91 .06
6.7
49
6.6
122.5
5-65
245-
4-55
SOLUBILITY OF ETHYL ETHER IN AQ. SALT SOLUTIONS AT 28°.
(Thorin, 1915.)
Gms.
S^vent. £*£0
Solvent.
Gms. Gms.
(CtfM> Solvent (QH5)20
per 100 cc. per 100 cc.
Solvent.
Solvent.
Solvent.
Water
5-85
o.s«Na3PO4
4-
17
o.5«NaSuccinate
4
.68
0.5 wNal
5-70
o . 5 n Na3 AsO4
4-
20
o. 5 wNa Citrate
4
.19
o . 5 n NaBr
4.68
o.S«Hg(CN)2
5-
7i
o. 5 wNa Acetate
4
•IS
o.swNaCl
4.48
o . 5 n NHUNOs
5-
37
o . 5 n Na Tartrate
4
.12
o . 5 n NaF
4-iS
o . 5 n FeCls
5-
09
o.s«NaPhthalate
5
.88
o.swNa2SO4
4-30
o . 5 n Na2Cr2O7
4-
84
o . 5 n Na Cinnamate
6
.29
0.5 wNa2CrO4
4.22
o.s«FeSO4
4-
33
o.5«NaBenzoate
5
•99
o . 5 n Na2MoO4
4-39
o.5wAl2(S04)3
3-
95
o.5«NaSalicylate
6
•44
o.5wNa2WO4
4.12
o . 5 n Am. Oxalate 4 .
74
o . 5 n Na Benzene Sulf onate
6
•°S
SOLUBILITY OF ETHYL ETHER IN 0.91 PER CENT (PHYSIOLOGICAL NORMAL
SALINE) AQUEOUS NaCl SOLUTION.
' (Bennett, 1912.)
Determinations made by freezing-point method. Ether of di6 = 0.720 used.
t".
Gms. (QH^O
per 100 Gms.
cc. (C2H5)20
(at 15 ) per 100
Aq. NaCl.
cc. Aq. NaCl.
0
13.08
18.27
5
11.15
I5-58
10
9-45
13.20
15
8.10
11.31
20
6.87
9.60
25
5.96
8.33
30
5-30
7.40
Purified ether prepared from methylated spirit gave slightly higher results.
SOLUBILITY OF ETHYL ETHER IN AQ. SULFURIC ACID AT o°.
(Kremann, igioa.)
Gms. per too Gms. Homogeneous Mixture.
Gms. per 100 Gms. Homogeneous Mixture.
(C2H5)20.
24.2
24.8
43-9
34
H20.
34-5
35-4
15.7
26.1
H2S04.
41-3
39-8
40.4
39-9
(C2H6)20.
16.1
6.1
53-8
H20.
42-7
78
8-5
H2S04.
41.2
15-9
37-7
Data for the system ethyl ether, ethyl alcohol, water, sulfuric acid at o° are also
given.
299 ETHYL ETHER
SOLUBILITY OF ETHER IN AQUEOUS ETHYL ALCOHOL AND IN AQUEOUS
METHYL ALCOHOL MIXTURES AT 20°.
(Bancroft, 1895.)
In Ethyl Alcohol. In Methyl Alcohol.
Per 5 cc. QHsOH. Per 5 cc. QHjOH. Per i cc., CHaOH. Per i cc. CH3OH.
'cc. H2O.*
cc. (Q
.VCC.HA* cc.
(QH6)20.f
cc. H2O.
cc. (C2HB)2O.
cc. H20.
cc. (C2HB),0.
50
I .
30
4.45
7
10
I.I3
0.83
I.
80
25
I.
70
4
7
,8
7
0.85
0.64
3
10
2.
3-87
8
4
0.60
0.52
5
8
3-
35
3.10
10
2
•5
0.56
0.44
10
6
5-
10
2.08
15
I
.8
0.63
0-45
IS
5.21
6
1.77
17
•5
I
1.23
* Saturated with ether.
f Saturated with water.
THE SYSTEM ETHYL ETHER-MALONIC ACID- WATER AT 15°. (Kiobbie, 1897.)
Results for Conjugated Liquid Layers Formed Results for the Liquid Layers in
when Insufficient Malonic Acid to Satu- Contact with Excess of
rate the
Gms. per 100 Gms
Layer.
Solutions Was Present.
. Lower Gms. per 100 Gms.
Layer.
Upper
Gms
Malonic Ac
, per 100 Gms.
Liquid.
id.
Solid Phase.
Malonic Add
«
«
tt
tt
tt
tt
it
Malonic
Acid.
0
4-63
II. 60
20.45
27-43
33-63
34-17
3I.II
H20.
92.23
87.42
79.92
69-S5
60.57
47-45
35-8i
26.76
Ethyl
Ether.
7-77
7-94
8.48
9.99
12
18.80
30.02
42.12
Malonic
Acid.
o
0.72
2.19
5.01
9-52
21.89
3° -44
31.11
HA
1. 2O
i-54
1.99
3-o8
5-i9
13-42
25-37
26.76
Ethyl
Ether.
98.80
97-74
95-82
91.91
85.29
64.91
44.19
42.12
Malonic
Acid.
8
9.96
19.41
27.22
35-51
46.48
51-33
57-37
H20.
0
0.42
2-79
5-23
10.73
20.86
26.30
39.10
Ethyl.
Ether.
92
89.61
77.80
67-54
53-75
32.66
22.36
3-52
Data for the system ethyl ether, succinic acid nitrile and water are given
by Schreinemakers, 1898.
Data for the extraction of formic acid from water by ether are given by Dakin,
Janney and Wakemann, 1913.
ETHYL FORMATE HCOOC2H6.
100 grams water dissolve 10 grams ethyl formate at 22°. (Traube, 1884.)
ETHYL METHYL KETONE CH3.CO.C2H6.
SOLUBILITY IN WATER. (Rothmund; 1898.)
By synthetic method, see Note, page 16.
,0 Gms. Ketone per 100 Gms. Gms. Ketone per 100 Gms.
Aq. Layer. Ketone Layer. Aq. Layer. Ketone Layer.
-io 34.5 89.7 90 16.1 84.8
+ 10 26.1 90 no 17.7 80
30 21.9 89.9 130 21.8 71.9
50 17.5 89 140 26 64
70 16.2 85.7 i5i.8(crit. temp.) 44. 2
The accuracy of Rpthmund's data is questioned by Marshall (1906) and the
following new determinations given.
t'. 64.7°. 65.5°- 73-6°. 91-0°. 15°. 73-6°.
Wt. % Ketone in Mixture 18.15 18.08 18 18.08 88.2 85.05
Data for the reciprocal solubility of ethyl methyl ketone and water, containing
J-5% ethyl alcohol, are given by Bruni (1899, 1900). This system is of interest
particularly on account of having both an upper and a lower critical point.
Freezing-point data for mixtures of ethylmethyl ketone and water are given by
Timmermans (1911) and by Bruni, 1899, 1900.
ETHYL KETONE 300
DiETHYL KETONE (Propione) (C2H6)2CO.
SOLUBILITY IN WATER. (Rothmund, 1898.)
The determinations were made by Synthetic Method, see p. 16. The critical
temperature could not be reached and high accuracy is not claimed for the results.
Cms. Diethyl Ketone Cms. Diethyl Ketone
t». per IPO Gms. t°. per ioo Cms.
Aq. Layer. Ketone Layer. Aq. Layer. Ketone Layer.
20 4.60 ... loo 3.68 93 .10
40 3-43 97-42 120 4.05 QO.lS
60 3.08 96.18 140 4.76 87.01
80 3.20 94.92 160 6.10 83.33
ETHYL PROPIONATE C2H6COOC2H5.
SOLUBILITY IN WATER AND IN AQUEOUS ETHYL ALCOHOL MIXTURES.
(Pfeiffer, 1892; Bancroft, 1895.)
. 4i™v,r,i cc. H2O to Cause Separation of a Second Phase in
F M- ? Mixtures of the Given Amounts of Alcohol
and 3 cc. Portions of Ethyl Propionate.
3 2.32
6 6.87
9 12.35
12 IQ-I?
15 27.12
18 36.84
21 50.42
24 CO
100 grams H2O dissolve 1.7 grams ethyl propionate at 22°. (Traube, 1884.)
DiETHYL Diacetyl TARTRATE (CHOCOCH3)2(COOC2H6),.
Freezing-point lowering data (solubility, see footnote, p. i) for mixtures of
diethyl diacetyl tartrate and each of the following compounds are given by
Scheuer (1910); m nitrotoluene, ethylene bromide, phenol and naphthalene.
Results for diethyl diacetyl tartrate and naphthalene are also given by Palazzo
and Batelli (1883).
ETHYL VALERATE C4H9COOC2H6.
ETHYL (Iso) VALERATE (CH3)2.CH.CH2COOC2H6.
SOLUBILITY OF EACH IN WATER AND IN AQUEOUS ALCOHOL MIXTURES AT 20°.
(Pfeiffer, 1892; Bancroft, 1895.)
ioo cc. water dissolve 0.3 .cc. ethyl valerate at 25°.
100 cc. water dissolve 0.2 cc. ethyl iso valerate at 20°.
ioo cc. ethyl iso valerate dissolve 0.4+ cc. water at 20°.
Mixtures of Ethyl Alcohol, Mixtures of Ethyl Alcohol,
Ethyl Valerate and Water. Ethyl Iso Valerate and Water.
Per 5 cc. Ethyl Alcohol.
CC.Alcohol* cc.H20.f cc.Alcohol* cc.H2O-t ' 177 "Cc Ethyl '
CC'H2°- Iso Valerate.
10 0.15
8 0.23
6 0.46
5 o-72
4 1.23
* cc. Alcohol in mixture.
t cc. H2O added to cause the separation of a second phase in mixtures of the given amounts of alcohol
and 3 cc. portions of ethyl valerate.
3
1.42
39
53-13
9
7.18
45
63.60
15
14-13
57
90-53
21
22.40
72
131.0
27
31.62
81
180.0
33
41 .62
ETHYLENE C2H4.
301 El
SOLUBILITY IN WATER AND IN ALCOHOL.
(Bunsen and Carius; Winkler, 1906.)
t°.
O
0
0.
.226
O
q-
.0281
Solubility
in Alcohol.
5
O
.191
0
.0237
t°. I(^c
Vol^AlcSd.
10
0
.162
o
.0200
0
359-5
15
0
•139
0
.0171
4
337-5
20
0
.122
0
.0150
10
308.6
25
0
.108
o
.0131
15
288.2
30
o
.098
0
.0118
20
271-3
ETHYLENE
O.I.
0.25.
0.5.
0.75.
X.O.
0.154
0.144
0.130
0.118
o . 1056
0.153
0.144
0.128
0.114
O.IOI
0.157
0.156
o.i55
0.154
0.1525
0.1425
0.127
0.109
0.093
For ft and q see Ethane, p. 285.
SOLUBILITY OF ETHYLENE IN AQUEOUS SOLUTIONS OF ALKALI HYDROXIDES,
ETC., AT 15°. (Billitzer, 1902.)
Results in terms of the Ostwald Solubility Expression /. See p. 227.
Solubility 1K in Aq. Solution of Normality:
Aqueous Solution of:
KOH
NaOH
NH40H
| Na2SO4
In HzO alone o . 1593
SOLUBILITY OF ETHYLENE IN METHYL ALCOHOL AND IN ACETONE. (Levi, 1901.)
Results in terms of the Ostwald Solubility Expression /. See p. 227.
t°. In Methyl Alcohol. In Acetone. t". In Methyl Alcohol. In Acetone.
o 3-3924 4-0652 30 1.8585 1.8680
10 2.8831 3-358° 40 1-3432 1.0852
20 2.3718 2.6278 5O 0.8259 0.2772
25 2.1154 2.2500 60 0.3506
The formulas from which the above figures were calculated are:
In Methyl Alcohol, I = 3 .3924 — 0.05083 / — o.ooooi ^.
In Acetone, / = 4.0652 — 0.06946 / — 0.000126 P.
SOLUBILITY OF ETHYLENE IN SEVERAL SOLVENTS. (McDaniel, 1911.)
qnlvwi *° Abs- Coef- Bunsen Qnlv^nt t « Abs- Coef- Bunsen
Solvent. t. A Coef.0. solvent. t. A Coef . 0.
Benzene 22 3.010 2.786 Heptane 22.4 3-463 3.207
35 2.655 2.353 35 3-186 2.824
50 2.482 2.100 39 3.110 2.722
Hexane 22 3.038 2.8141 Acetone 20 2.571 2.290
35 2.826 2.505 35 2.308 2.046
? " 45 2.586 2.219 Limonene 22 no constant equilibrium
Abs. Coef. A = vol. of ethylene absorbed by unit vol. of solvent at temp, stated.
For definition of Bunsen Coef. ft, see carbon dioxide, p. 227.
The Coef. of Abs. ft of ethylene in Russian petroleum is o. 1 64 at I o° and o. 1 42 at 20°.
(Gniewosz and Walfisz, 1887.)
Freezing-point data (solubility, see footnote, p. i) for mixtures of ethylene and
methyl ether are given by Baume and Germann, 1911, 1914.
ETHYLENE BROMIDE C2H4Br2.
F.-PT. DATA FOR MIXTURES OF ETHYLENE BROMIDE AND OTHER COMPOUNDS.
Ethylene Bromide + Naphthalene (Baud, 1912; Dahms, 1895.)
44 + ft Naphthol (Bruni, 1898.)
• " -j- " + Picric Acid (Bruni, 1898.)
-j- Paraldehyde (Paterno and Ampola, 1897.)
-j- Phenol (Dahms, 1895; Paterno and Ampola, 1897.)
-j- Toluene (Baud, 1912.)
" + Bromotoluene (Paterno and Ampola, 1897.)
"- " +£Xylene
ETHTLENE CYANIDE 302
ETHYLENE CYANIDE C2H4(CN)2.
DISTRIBUTION BETWEEN WATER AND CHLOROFORM. (Hantzsch and Vagt, 1901.)
Gm. Mols. QjH^CCN);; per Liter. . Cl.
* • / T r^-w-rf^i -T Ivatio. ~— •
Aq. Layer, c\. CHClj Layer, c%. c2.
o 0.0786 0.0464 1.69
10 0.0787 0.0463 1.70
20 0.0791 0.0459 1.72
Additional data for the influence of KOH, KC1 and HC1 on the above distri-
bution are also given.
DiETHYLENE ETHER (CH2OCH2)2.
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
diethylene ether and water, by Unkovskaja, 1913.
Tetraphenyl ETHYLENE (C6H5)2C:C(C6H5)2.
Freezing-point data for tetraphenyl ethylene + silicotetraphenyl are given by
Pascal and Normand (1913).
0 EUCAINE Ci5H21NO2 and Salts.
100 cc. H2O dissolve 0.296 gm. anhydrous ft eucaine at 20°. 1 (Zalai,
100 cc. oil of sesame dissolve 3.49 gms. anhydrous ft eucaine at 20°. ) 1910.)
100 cc. aniline oil dissolve 66.6 gms. anhydrous /3 eucaine at 20°.
100 cc. H2O dissolve 2.5 gms. /3 eucaine hydrochloride at 15-20°
(Squire and
Caines,
1905.)
ioo cc. 90% alcohol 9
100 cc. H2O " 25 " lactate
ioo cc. 90% alcohol " 12.5 "
loocc. CHC13 " 20 "
EUROPIUM Bromonitrobenzene SULFONATE Eu[C6H3Br(i)N02(4)SO3(2)]j.-
ioH2O.
ioo gms. sat. solution in water contain 6.31 gms. anhydrous salt at 25°.
(Katz and James, 1913.)
FATS.
SOLUBILITY OF THE FATTY ACIDS OBTAINED FROM SEVERAL SOURCES IN
ALCOHOL AND IN BENZENE. (Dubois and Fade, 1885.)
Crude Fatty
Gms. Fat j
>er ioo Gms. Ab;
5. Alcohol at:
Gms. Fats per ioo
Acid of:
r o°.
10°.
26°.
Gms. Benzene at 1 2°,
Mutton
2.48
5.02
67.96
14.70
Beef
2.51
6.05
82.23
15.89
Veal
5
13.78
137.10
26.08
Pork
5-63
11.23
118.98
27.30
Butter
10. 61
24.81
158.2
69.61
Margarine
2-37
4-94
47.06
13-53
MlSCIBILITY OF FATS AND 90 VOL. PER CENT ALCOHOL AT 37°. (Vandevelde, 1911.)
Mixtures of fats and alcohol in various proportions were shaken twice daily for
8 days and the volume of each layer, as well as its composition, determined.
Composition of Mixture-
Mixture. . — * .
cc. Alcohol cc. Fat
Alcohol + Cocaline 25 5
Volume after Agitation.
Gms. Fat per Gms. Alcohol
ioo Gms. per ioo Gms.
\lcohol Layer Fat Layer.
4-9 19-4
cc. Alcohol
25-4
cc. Fat ,
4-6
«
(1
2O
IO
19
.2
10.8
5
.6
16
,2
it
u
is
IS
13
17
7
.2
13
5
N
((
10
20
6
•7
23
•3
9
.1
12
,2
ft
ll
5
25
i
.1
28
•9
13
II,
4
Alcohol +
Butter Fat
25
5
25
.r
4
•9
3
• 5
17
4
"
"
20
IO
19
.2
IO
.8
3
•5
14
i
"
"
IS
IS
13
17
4
14
i
"
**
10
20
7
. i
22
9
S
• 7
"
"
5
25
2
28
14
.1
9
5
Alcohol +
Olive Oil
25
S
24
• 7
5-3
2
•3
ii
2
"
"
20
IO
19
.2
IO
.8
2
•4
8
.7
'*
"
IS
15
13
17
2
• 4
8
7
N
«
10
20
7
-5
22
• 5
2
• 5
• 8
8
H
M
5
25
2
.2
27
.8
7
7
,6
For other data on the solubility of fats see Ewers (1910) and Louise (1911).
303 FLUORENE
FLUORENE (Diphenylenemethane) C6H4.CH2.C«H4.
Freezing-point data (solubility, see footnote, p. i) are given by Kre*mann (1911)
for mixtures of fluorene and each of the following compounds: o, m and p dintro-
benzene, 1.3.5, trinitrobenzene, dinitrophenol, dinitrotoluene, trinitrotoluene and
picric acid.
FLUORESCEIN
100 gms. H2O dissolve 0.005 Sm« fluorescein at 20-25° (Dehn, 1917.)
100 gms. pyridine dissolve 13.29 gms. fluorescein at 20-25° "
100 gms. aq. 50% pyridine dissolve 37.22 gms. fluorescein at 20-25° "
FORMALDEHYDE, Solid Polymers (CH2O)n.
SOLUBILITY OF THE Six WELL-DEFINED SOLID POLYMERS OF FORMAL-
DEHYDE IN WATER. (Auerbach and Barschall, 1908.)
Name. Formula. m. pt. Gms. per 100 cc. Sat. Solution in Water.
Paraformaldehyde (CH2O)n+#H2O 150-160 20-30 gms. at 18°
a Polyoxymethylene (CH2O)n 163-8 n gms. at 18-25°
/3 Polyoxymethylene (CH2O)n 163-8 3.3 gms. at 18°, about 4 at 25°
7 Polyoxymethylene (CH2O)n ^S~5 less than o.i at 18°, o.i gm. at 25°
8 Polyoxymethylene (CH2O)n 169-70 practically insoluble
a Trioxymethylene C3H6O3 63-4 17.2 at 18°, 21.1 at 25°
All are insoluble in alcohol and ether except trioxymethylene.
SOLUBILITY OF TRIOXYMETHYLENE IN AQ. SODIUM SULFITE SOLUTIONS AT 15°.
(Lumiere and Seyewetz, 1902.)
Gms. Na2S03 per 100 cc. H2O 5 10 20 25 28 (sat.)
Gms. CsHeOs per 100 cc. sat. sol. 22 24 26 27 27
Data are also given for the solubility of various mixtures of trioxymethylene
and sodium sulfite in water at 15°.
The distribution coefficient of formaldehyde between water and ether is 8.5 at
O° and 9.23 at 2O°. (Hantzsch and Vagt, 1901.)
FORMAMIDE HCONH2.
SOLUBILITY IN WATER, DETERMINED BY THE FREEZING-POINT METHOD.
(English and Turner, 1915.)
Gms. Gms. Gms.
t° of HCONH2 Solid t° of HCONH2 <, r , p, ^ t° of HCONH2 ~ ,. . p.
Solidif. per 100 Phase. Solidif. per 100 Solid Phase. Solidif per IQQ 2 Solid Phase.
Gms. H2O. Gms. H2O. Gms. H2O.
— o o Ice —31.1 116.4 Ice —37-6 267 HCONHa
-2.7 9.93 " -42.5 169 -29.4 369-8
-5.7 17.87 " -45-4 187-8 HCONH2.H2O -21.9 540.3
-ii 35.45 " -40.4 218.3 " -14-5 836.8
-23.6 81.93 -40 241.4 - 6.4 1780
Similar data are also given for formamide + formic acid and formamide -h
propionic acid.
o and p ChloroFORMANILIDES C1.C6H4NH.CHO.
Freezing-point lowering data for mixtures of o and p chloroformanilide are
given by King and Orton, 1911.
FORMIC ACID HCOOH.
SOLUBILITY IN WATER, DETERMINED BY FREEZING-POINT METHOD. (Faucon, 1910.)
to f Gms. HCOOH «, . Gms. HCOOH to of Gms. HCOOH
o o
-5 12.5
— 10 23
— 15 32
— 20 39.2
-25 46.5
Similar data for mixtures of 97.4% formic acid and water are given by Kremann,
1907.
-30
53
-40
74.2
-35
57-6
-30
79
-40
62.5
— 20
84.2
-45
66.5
— 10
89.4
—49 Eutec.
70
0
95
-45
71.7
+8.51
TOO
FORMIC ACID 304
DISTRIBUTION OF FORMIC ACID BETWEEN WATER AND BENZENE AT 13-15°.
(v. Georgievics, 1913.)
A small separatory funnel was used and the acid in each layer titrated with o.i
n NaOH, using phenolphthaleine as indicator.
Cms. HCOOH Found per: Cms. HCOOH Found per:
25 cc. H2O Layer.
isocc. C6H6 Layer.
25 cc. H2O Layer.
iSoce. C6H6 Layer.
1.016
0.016
2.365
0.035
1-539
0.031
3.826
O.O62
1.800
0.024
5^74
O.II4
2. 112
0.031
7.836
0.138
p__
The distribution ratio of formic acid between water and benzene was found by
King and Narracott (1909) to be I to 0.0242 at room temp.
Freezing-point lowering data (solubility, see footnote, p. i) are given for mix-
tures of formic acid and dimethylpyrone by Kendall, 1914.
FUMARIC ACID COOH.CH:CH.COOH.
MALEIC ACID COOH.CHrCH.COOH. (See also p. 398.)
SOLUBILITY IN WATER. (Vaubel, 1899.)
loo gms. water dissolve 0.672 gm. fumaric acid at 165°.
100 gms. water dissolve 50 grams maleic acid at 100°.
Data for the distribution of fumaric acid between water and ether at 25° are
given by Chandler, 1908.
FURFUROL C4H3OCHO.
SOLUBILITY IN WATER. (Rothmund, 1898.)
Determinations by Synthetic Method, for which see p. 16.
Gms. C4H3OCHO per 100 Gms. Gms. C4H3OCHO per 100 Gms.
Aq. Layer. Furfurol Layer. Aq. Layer. Furfurol Layer.
40 8.2 93.7 ioo 18.9 83.5
50 8.6 93 no 24 78.5
60 9.2 92 115 28 74.6
70 10.8 90.7 120 34.4 68.1
80 13 89 122.7 (crit. t.) 51
90 15.5 86.6
GADOLINIUM CobaltiCYANIDE GdiCCoCeNe^HjO.
looo gms. aq. 10% hydrochloric acid dissolve 1.86 gms. of the salt at 25°.
(James and Willard, 1916.)
GADOLINIUM GLYCOLATE Gd2(C2H3O3)3.2H2O. ,
IOOO CC. H2O dissolve 14.147 gms. of the salt at 2O°. (Jantsch and Grunkraut, 1912-13.)
GADOLINIUM Magnesium NITRATE, etc.
SOLUBILITY OF DOUBLE NITRATES OF GADOLINIUM AND OTHER METALS IN CONC.
NITRIC ACID OF dy = 1.325 ( = 51.59 GM. HNO3 PER ioo cc.) at 16°. (Jantsch, 1912.)
Gms. Hydrated
Salt. Formula. Salt per Liter
Sat. Solution.
Gadolinium Magnesium Nitrate [GdCNOa^feMga^I^O 352 .3
Nickel " " Ni3 " 400.8
Cobalt " " Co3 " 451-4
Zinc Zn3 " 472.7
GADOLINIUM OXALATE Gd2(C2O4)3.ioH2O.
SOLUBILITY IN AQUEOUS SOLUTIONS OF SULFURIC ACID AT 25°. (Wirth, 1912.)
Normality of Gms. per ioo Gms. Sat. Sol.
Aq-H2S04. — Gd^ Gd2(CA)3.
2.16 0.1883 0.3005 Gd2(C204)3.ioH2O
3.11 0.3010 0.4803
4-32 0.4359 0.6956
6.175 0.707 1.128
305 GADOLINIUM OXALATE
SOLUBILITY OF GADOLINIUM OXALATE IN AQUEOUS 20% SOLUTIONS OF
METHYLAMINE OXALATE, ETHYLAMINE OXALATE AND TRIETHYLAMINE OXALATE.
(Grant and James, 1917.)
.
Aq. 20% Methylamine Oxalate 0.069
" Ethylamine 0.360
" Triethylamine " 0.883
GADOLINIUM Dimethyl PHOSPHATE Gd2[(CH3)2PO4]6,
100 gms. H2O dissolve 23 gms. Gd2[(CH3)2PO4]6 at 25° and 6.7 gms. at 95°.
(Morgan and James, 1914.)
GADOLINIUM SULFATE Gd2(SO4)3.8H2O.
SOLUBILITY IN WATER. (Benedicks, 1900.)
t<>. , Gms- era8 H2bPef I0° Solid Phase'
• o 3.98' ' Gd2(SO4)3.8H2O
10 3-3
14 2.8
25 2.4
34.4 2.26
SOLUBILITY OF GADOLINIUM SULFATE IN AQUEOUS SOLUTIONS OF:
Sodium Sulfate at 25°. (Bissell and James, 1916.) Sulf uric Acid at 25°. (Wirth, 1912.)
Gms. per 100 Gms. H2O. Normality Gms. P61" I0° Gms- Sat- So1-
'
NasS04.
O
Gd2(SO4)
2.15
Gd2
UUU i 1UIOC.
(SO4)3.8H2O
ofH
0
' Gd203 =
1-793
2,
Igsl*
Gd2(S04)3.8H20
0.43
2.06
it
0
I
1.98
3
.291
M
0.47
0.76
Gd2(SO4)3.Na2SO4.2H2O
o.
505
2-365
3-
931
M
1.26
0.17
11
I,
I
2.29
v5
.807
€(
3-01
0.07
ti
2
.16
1.789
2
974
tl
7.46
0.05
(i
6.
175
0.528
0.8777
it
27.40
0.05
(i
12.
6
0.0521
O.
,0867
ft
GADOLINIUM SULFONATES.
SOLUBILITY IN WATER. Gms
Salt. Formula. *°-&SK?S Authority-
Gms. H2O.
xS 43.8
Gd[CtH3Br(N02)SOs(I.4.2)],IoH20 ,S 6.3.
GALACTOSE C6Hi2O6. See also Sugars, pages 695-7.
100 gms. saturated solution in pyridine contain 5.45 gms. C6Hi2O6 at 26°,
density of solution = 1.0065. (Holty, 1905.)
100 gms. H2O dissolve 68.3 gms. galactose at 20-25°. (Dehn, 917.)
100 gms. aq. 50% pyridine dissolve 6.83 gms. galactose at 20-25°. "
GALLIC ACID 3.4.5, (OH)3C6H2COOH.H2O.
SOLUBILITY IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Wt. PerCent fnT^nntPfr n Wt. Per Cent rniS"™™?'*? O
CjHsOHm ^Sat-So.. <°^™GH*»° &H£H in ^of Sat. Sol. «*>*%$£?
Solvent. Sat. Sol. Solvent. Sat ^
o 1.002 1.15 60 0.957 16
10 0.992 2 70 0.946 18
20 0.983 4.2 80 0.933 I9-9
30 0.977 7.5 90 0.919 21.2
40 0.972 10.6 95 0.911 21.6
50 0.965 13.4 IOO 0.902 22.2
IOO gms. H2O dissolve 0.95 gm. gallic acid at 15°. (Greenish and Smith, 1903.)
loo gms. H2O dissolve 33. 3 gms. gallic acid at 100°. (U. S. P. VIII)
GALLIC ACID 306
SOLUBILITY OF GALLIC ACID IN ORGANIC SOLVENTS AT 25°.
(Seidell, 1910.)
^ «f Qof Gms- CfiH2(OH)j
Solvent. Density of Solvent. Solution COOH.H2O per 100
Gms. Sat. Sol.
Acetone du> = 0.797 0.941 25-99
Amylalcohol (iso) ^0=0.817 o . 834 5.39
Amylacetate ^20 = 0.875 0.878 2.72
Benzene d& = 0.873 °-&7S 0.022
Carbon Bisulfide di = 1.258 1.262 0.042
Ether (abs.) ^20 = 0.711 0.718 i-37°
Ethylacetate d& = 0.892 0.911 3.610
The amount of gallic acid dissolved by carbon tetrachloride, chloroform and
toluene was too small for estimation.
100 gms. glycerol dissolve 8.3 gms. C6H2(OH)3CpOH.H2O at 25°. (U. S. P. VIII.)
loo gms. 95% formic acid dissolve 0.56 gm. gallic acid at^!9.4°. (Aschan, 1913.)
GERMANIUM DIOXIDE GeO2.
loo gms. H2O dissolve 0.405 gm. GeO2 at 20°, and 1.07 gms. at 100°. (Winkler, 1887.)
GERMANIUM (Mono) SULFIDE GeS
GERMANIUM (Di) SULFIDE GeS*
100 gms. H2O dissolve 0.24 gm. GeS
loo gms. H2O dissolve 0.45 gm. GeSa. (Winkler, 1887.)
GLASS.
For data on the solubility of glass in water and other solvents, see:
(Cowper, 1882; Emmerling, 1869; Bohling, 1884; Kreusler and Herzhold, 1884; Kohlrausch, 1891;
Forster, 1892; Mylius and Forster, 1889; 1892; Wartha, 1885; Nicolardot, 1916.)
GLOBULIN (Serum).
SOLUBILITY IN AQUEOUS MAGNESIUM SULFATE SOLUTIONS.
(Galeotti, 1906; Scaffidi, 1907.)
The precipitated globulin (from oxblood) was not dried, but pressed between
filter paper, and an excess introduced into each MgSC>4 solution. After constant
agitation for 12 hours, the saturated solution was filtered, weighed and evaporated
to constant weight, the coagulated globulin then washed to disappearance of SO4
and dried and weighed.
Results for 10°. Results for 25°. Results for 40°. Results'for 55°. Results for 70°.
Gms. per ido Gms. Gms. per 100 Gms. Gms. per 100 Gms. Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol. Sat. Sol. Sat. Sol. Sat. Sol. Sat. Sol.
MgS04.
Globulin.
MgS04.
Globulin.
MgS04.
Globulin.
MgS04.
Globulin.
MgS04.
Globulin.
0.06
0.07
0.06
0.07
0.06
0.42
0.40
1.14
0.71
o-34
0.18
0-34
O.2I
0.61
0.31
1.42
0.88
2.14
2.52
o-55
0.65
I.63
0.63
2. 2O
0.61
5-39
i. 60
3-34
4-74
1.14
2. II
3-35
2.28
5.56
1.92
8.31
S-64
5-06
6.83
1.17
4-32
4-42
3-35
6.07
5-40
8.63
10.81
3.10
9.22
1.76
I3-63
2.60
16
4-03
14.72
3
13-84
2. II
13.29
i
20.86
0.37
21.30
o-95
18.47
i. 02
17.90
0.69
15.38
0-37
24.18
0.18
25-47
0.03
27.03
O.OI
17.67
0.07
The coagulation curve and freezing-point curve are also given.
GLUCOSE d C6Hi2O6.H2O. See also Sugars, pages 695-7.
100 gms. H2O dissolve 82 gms. glucose at 20-25°. (Dehn, 1917.)
100 gms. pyridine 7.62 "
100 gms. aq. 50% pyridine " 49.17 " " " "
100 gms. trichlor ethylene 0.006 " 15°
(Wester and Bruins, 1914.)
GLUTAMINIC ACID C3H5NH2(COOH)2.
Data for the solubility of glutaminic acid in aq. salt solutions are given by
Wiirgler (1914) and Pfeiffer and Wurgler (1916).
307 GLUTAMINIC ACID
GLUTAMINIC ACID HYDROCHLORIDE C3H6NH2(COOH)2.HC1.
SOLUBILITY IN WATER. (Stoitzenberg, 1912.)
(The following results were taken from the diagram given by the author.)
Cms. Glutaminic Acid. Cms. Glutaminic Acid.
t°. HC1 per 100 cc. t°. HC1 per 100 cc.
Sat. Sol. Sat. Sol.
o 3i-5 60 57
10 34.5 70 62
20 38 80 67.5
30 42-5 90 74
40 47 100 81
50 52 20 1.4 (sol. sat. with HC1)
GLUTARIC ACID (Pyrotartaric) (CH2)3(COOH)2.
SOLUBILITY IN WATER. (Lamouroux, 1899)
t°. o°. 15°. 20°. 35°. 50°. 65°.
Cms. (CH2)3(COOH)2
per 100 cc. solution 42.9 58.7 63.9 79.7 95.7 ni.8
100 gms. 95% formic acid dissolve 55.62 gms. glutaric acid at 18.6°. (Aschan, 1913.)
Data for the distribution of glutaric acid between water and ether at 25° are
given by Chandler, 1908.
F. pt. data for glutaric acid + sulfuric acid. (Kendall and Carpenter, 1914.)
GLYCINE (Glycocoll) CH2.NH2.COOH.
loo gms. H2O dissolve 51 gms. CH2.NH2.COOH at 20-25°. (Dehn, 1917.)
100 gms. pyridine dissolve 0.61 gm. CH2.NH2.COOH at 20-25°.
100 gms. aq. 50% pyridine dissolve 0.74 gm. CH2.NH2.COOH at 20-25°. "
SOLUBILITY OF GLYCINE IN WATER AND IN AQ. SALT SOLUTIONS AT 20°.
(Pfeiffer and Wurgler, 1915, 1916.)
Mnlc Sal* Gms. Glycine ,» , colf Gms. Glycine
Water only 1.962 LiCl 0.96 4.188
BaCl2 0.5 2.375 LiBr 0.97 4.245
BaBr2 0.5 2.954 SrCl2 0.25 2.129
SrCl2 0.5 2.362 0.50 2.331
SrBr2 0.49 2.440 i 2.605
CaCl2 0.57 4.848 2 3.301
CaBr2 0.51 4-994
10 cc. sat. aq. solution contains 1.8 gms. glycine + 2.7 gms. KC1 at 20° when
both are present in the solid phase. (Pfeiffer and Modelski, 1912.)
GLYCOLIC ACID CH2OH.COOH.
SOLUBILITY IN WATER. (Emich, 1884.)
t°. 20°. 60°. 80°. 100°.
Gms. CH2OH(COOH)
per 100 gms. H2O 0.033 0.102 0.235 0.850
PhenylGLYCOLIC ACID dextro and racemic. CH.C6H5.OH.COOH.
SOLUBILITY OF DEXTRO AND OF RACEMIC PHENYL GLYCOLIC ACID IN CHLOROFORM.
(Holleman, 1898.)
Gms. Detro Acid Gms. Racemic
t°. per loo Gms. t°. Acid per 100
CHC13. Gms. CHClj.
IS 0.952 IS 0.877
25 1.328 25 1.07
35 i-95o 35 1-6°
GLYCYRRHIZIC ACID.
100 gms. sat. solution in H2O contain 0.575 gm. glycyerrhizicacid at 15°. (Capin, '12.)
IOO gms. sat. solution in H2O contain 0.152 gm. Am. glycyrrhizate at o° and
0.225 gm- at 15°. ' (Capin, 1912.)
PhenylGLYOXAL Phenyl hydrazone C6H5.CO.CH.N.NH.C6H6.
One liter C6H6 dissolves 52.6 gms. of the A form at 5°. (Sidgwick, 1915 )
One liter CeHe dissolves 2.9 gms. of the B form at 5°. "
GOLD 308
GOLD Au.
SOLUBILITY OF GOLD IN POTASSIUM CYANIDE SOLUTIONS. (Maclaurin, 1893.)
Gold disks were placed in Nessler tubes with aqueous KCN solutions.
Gms. Au Dissolved in 24 Hours in Nessler Tubes:
rer cent
KCN.
Full.
£ Full.
Oxygen.
Passed in.
Oxygen +
Agitation.
O.I
I
5
O.OOI95
O.OOI62
0.0032
0.00331
O.OO4I8
0.0046
o . 00845
0.01355
0.0472
20
5°
O.OOI2
O.OOO43
0.00305
O.OOO26
O.OII5
0.00505
0.0314
O.OIO8
The following data for more dilute KCN solutions are given by Christy (1901).
Gold strips 2 X | inch were rotated for 24 hrs. in aq. KCN solutions and the
loss in weight determined.
1 Per cent Mgs. Au Per cent Mgs. Au Per cent Mgs. Au
KCN. Dissolved. KCN. Dissolved. KCN. Dissolved.
o o.oio 0.002 0.44 0.016 74-96
0.0005 0.043-0.07 0.00325 1.77 0.0325 150.54
o.ooi 0.10-0.23 0.004 4-29 0.065 168.12
0.0016 0.16 0.008 48.43
Data are also given for 48 hour periods and for solutions containing Oa.
One liter of cone. H NOs dissolved o. 66 gm. Au on boiling for two hours. (Dewey, '10.)
Data for the rate and limit of solubility of Au in cone. HC1 solutions of iron
alum and of cupric chloride are given by McCaughey, 1909.
GOLD CHLORIDE (Auric) AuCl3.
100 gms. HaO dissolve 68 gms. AuCla.
When i gm. of gold as chloride is dissolved in aq. HC1 of different strengths and
the solutions shaken with 100 cc. portions of ether, the following percentages of
the gold enter the ethereal layer. With 20% HC1, 95%; 10% HC1, 98%; 5% HC1,
98%; 11% HC1, 84% and 0.18% HC1, 40.3% of the gold.
Distribution results, indicating considerable variation in the constitution of the
dissolved substance in the two layers, are also given. (Mylius, 1911.)
GOLD PHOSPHORUS TRI CHLORIDE (Aurous) AuClPCl3.
100 gms. PC13 dissolve i gram at 15°, and about 12.5 grams at 120°.
(Lindet — Compt. rend. 101, 1492, '85.)
GOLD ALKALI DOUBLE CHLORIDES.
SOLUBILITY OF SODIUM GOLD CHLORIDE, LITHIUM GOLD CHLORIDE,
POTASSIUM GOLD CHLORIDE, RUBIDIUM GOLD CHLORIDE, AND
CAESIUM GOLD CHLORIDE IN WATER.
(Rosenbladt — Ber. 19, 2537, '86.)
Grams Anhydrous Salt per 100 Grams Solution.
10
20
30
40
50
60
70
80
90
100
100 gms. glycerol (di6 = 1.256) dissolve 0.21 gm. AuK(CN)2.5H2O at 15-16°.
(Ossendowski, 1907 )
NaAuCU.
LiAuCU.
KAuCU.
RbAuCU-
CsAuCU.
58.2
53 -1
27.7
4-6
o-5
60.2
57-7
38.2
9-0
0.8
64.0
62.5
48.7
13-4
i .7
69.4
67-3
59-2
17.7
3-2
77-5
72.0
70-0
22.2
5-4
90.0
76.4
80.2
26.6
8.2
81.0
3I.O
12 .O
85-7
35-3
16.3
39-7
21-7
44.2
27-5
309 GUAIACOL
GUAIACOL C6H4(OH)OCH3(7.
GUAIACOL CARBONATE [C6H4(OCH3)O]2CO.
SOLUBILITY IN WATER, ALCOHOL, ETC. (u. s. P. vra.)
Cms. per 100 Cms. Solvent.
Solvent. t°.
Guaiacol. Guaiacol Carbonate.
Water 25 1.89
Alcohol 25 ... 2.08
Chloroform 25 ... 66.6
Ether 25 ... 7.69
Glycerol 25 100
The coefficient of distribution of guaiacol carbonate between olive oil and water
at 25° is given as Sr = 3.7 by Boeseken and Waterman, 1911, 1912.
Freezing-point lowering data (solubility, see footnote, p. i) are given for mix-
tures of guaiacol and a. naphthylamine by Pushin and Mazarovic, 1914; for mix-
tures of guaiacol and picric acid by Philip and Smith, 1905; and for mixtures of
guaiacol and salol by Bellucci, 1912, 1913.
a Tri PhenylGUANIDINE CeH.N:C(NHCaHO,.
SOLUBILITY IN MIXTURES OF ALCOHOL AND WATER AT 25°. (HollemanandAntusch,'94.)
Gms. Gms.
Vol. % C6H5N:C(NHC6Hfi)2 Density Vol. % C«H5N:C(NHC6H5)2 Density
Alcohol. per 100 Gms. of Solutions. Alcohol. per 100 Gms. of Solutions.
Solvent. Solvent.
ioo 6.23 0.8021 80 i. 06 0.8572
95 3.75 0.8158 75 0.67 0.8704
90 2.38 0.8309 70 0.48 0.8828
85 1.58 0.8433 6o °-22 0.9048
See remarks under a Acetnaphthalide, p. 13.
Freezing-point lowering data for mixtures of triphenylguanidine and triphenyl
methane and for triphenylguanidine and phthalide are given by Lautz, 1913.
HEMOGLOBIN.
ioo gms. H2O dissolve 15.16 gms. hemoglobin at 20-25°. (Dehn, 1917.)
ioo gms. pyridine dissolve 0.15 gm. hemoglobin at 20-25°. "
ioo gms. aq. 50% pyridine dissolve 0.77 gms. hemoglobin at 20-25°. "
HELIANTHIN (Methyl Orange, Tropaeolin).
ioo cc. H2O dissolve 0.0055 to 0.0225 gm. helianthin. (Dehn, igiya.)
ioo cc. pyridine dissolve 0.75 gm. helianthin. "
ioo cc. 50% aq. pyridine dissolve 62.5 gms. helianthin. "
Results for other solvents and observations on the state of colored compounds
in solution are given.
HELIUM He.
SOLUBILITY IN WATER, (von Antropoff, 1909-10.)
t°. Coef. of Absorption.
o 0.0134
IO O.OIOO
20 0.0138
30 0.0161
40 0.0191
50 0.0226
The coef. of absorption adopted for the present results is that of Bunsen as
modified by Kuenen. The modification consists in substituting unit of mass in
place of unit of volume of water, in the formula.
HELIUM
310
HELIUM He.
to
SOLUBILITY IN WATER.
(Estreicher — Z. physik. Chem. 31, 184, '99.)
Absorption Coefficient.
Cor. Barometic Vol. of
Pressure. Water.
Vol. of
He.
fl.
At Bar. Pressure
Minus H2O
Vapor Tension.
At 760 mm.
Pressure.
o
.000270
O
.0150
> 764
.0
73
•584
I
•093
O
.0149
O
.0149
758
.0
73
•578
I
.062
0
.000260
0
.0144
o
.0146
758
.0
73
•597
I
.046
0
•000255
0
.0142
O
.0144
757
.8
73
.641
I
.008
0
.000246
o
.0137
0
.0140
758
•4
73
.707
0
.996
0
.000242
0.0135
O
.0139
762
•3
73
•793
0
•983
0
.000238
o
•0133
o
.0137
764
•4
73
.897
0
•985
0
.000238
o
•0133
o
.0138
764
•5
74
.0167
0
.972
0
.000234
0
.0131
0
.0138
762
.0
74
.147
o
•957
o
.000232
o
.0129
0.0139
76l
•7
74
.294
0
•947
0
.000229
o
.0127
o
.0140
760
•9
74
.461
0
.920
0
.000223
o
.0124
0
.0140
5
10
IS
20
25
30
35
40
45
5o
For q and also absorption coefficient, see Ethane, p. 285.
HEPTANE n CH3(CH2)5CH3.
F.-pt. lowering data for mixtures of heptane and phenol are given by (Campett
and Delgrosso, 1913).
HEPTOIC ACID CH3(CH2)6COOH.
100 gms. H2O dissolve 0.241 gm. heptoic acid at 15°. (Lumsden, 1905.)
HEXAMETHYLENE (Hexahydrobenzene) . See Cyclohexane, p. 280.
HEXAMETHYLENE TETRAMINE (CH2)6N4.
100 gms. H2O dissolve 81.32 gms. (CH2)6N4 at 12°. (Delepine, 1895.)
ioo gms. abs. alcohol dissolve 3.22 gms. (CH2)6N4 at 12°. "
IOO CC. 90% alcohol dissolve 12.5 gms. (CH2)6N4 at I5-2O0. (Squire and Caines, 1905.)
T r\ri ^-»-v-« <-. /^t-1^1 *r1«si/i^1-«r«~k Q ^-w\ ^v, -.-»,. //~*LT \ XT *•»•*- -r/-»O /T^.I : _o«^\
ioo gms. CHC13 dissolve 8.09 gms. (CH2)6N4 at 12°.
HEXANE C6Hi4.
SOLUBILITY IN METHYL ALCOHOL.
(Rothmund, 1898.)
Determined by synthetic method, see p. 16.
t°.
(Delepine, 1895.)
Gms. Hexane per 100 Gms.
10
20
30
Alcoholic
Layer.
26.5
31.6
38.3
Hexane
Layer.
96.8
95-9
93-7
F.-pt. data for hexane + phenol.
Gms. Hexane per ioo Gms.
t°- Alcoholic Hexane
Layer. Layer.
35 43-6 9i-2
40 52-7 85.5
42.6 (crit. t.) 68.9
(Campetti and Delgrosso, 1913.)
HIPPURIC ACID C6H6CO.NH.CH2COOH.
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent
Water
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
50% Aqueous Pyridine
t°. C6H5CO.NHCH2COOH Authority,
per ioo Gms. Solvent.
20-25
0.42
(Dehn, 1917.)
22
9.80
(Timofeiew, 1894.)
22
5.20
"
23
2.80
"
20-25
88
(Dehn, 1917.)
3H HIPPURIC ACID
SOLUBILITY OF HIPPURIC ACID AT 25° IN AQUEOUS SOLUTIONS OF:
Formic Acid. (Kendall, 1911.) Sodium Hippurate. (Sidgwick, 1910.)
Normality Cms. Hippuric Normality Cms. Hippuric Normality of Cms. Hippuric
of Aq. Acid per of Aq. Acid per Aq. Sodium Acid per
HCOOH. Liter. HCOOH. Liter. Hippurate. Liter.
o 3.67 5 4-08 o 6.Q9(?)
1.25 3.61 10 4.77 i 13-9700
2-5 3-72
HIPPURIC ACID C6H6CONH.CH2COOH.
SOLUBILITY IN AQ. POTASSIUM HIPPURATE SOLUTIONS AT 20*.
(Hoitsema — Z. physik. Chem. 27» 3i?t '98.)
Density Gram Mols. per Liter Sol. Grams per Liter Solution. Solid
of Solutions. C9H9N03. KCgHgNCV C9H9NO3. 'KC9H8NO3.' Pnase-
.002 0.0182 O 3-276 0.0 CoHoNO,
.003 0.0163 o.on 2.919 2.39
.008 0.0183 0.071 3-278 15.43
.022 0.0234 0.254 4-191 55-lS
.114 0-064 1.36 11-47 295.4
.l82 O.I3I 2.21 23.46 480.1
192 0.147 2.32 26.32 504.1 iCeHjjNOg-f
195 0.153 2.40 27.40 52I.4J C9H^03.KC9H8N03.H»0
.201 0.133 2.50 23.82 543.1
.239 0.084 3.01 15.04 654.0
.282 0.068 3.57 1 2.l8 775-7
.282 0.065 3.58 II. 60 777-8) +KC9H8N03
1.276 0.031 3.56 5.55 773.4 KQtfsNOs
1.277 o.on 3.55 1.917 771.3
1.277 o-oo 3-56 ••• 773-4
HOLOCAINE HYDROCHLORIDE.
loo gms. H2O dissolve 2 gms. holocaine hydrochloride at 15-20°.
(Squire and Caines, .1905.)
HOMATROPINE HYDROBROMIDE Ci6H21NO3.HBr.
SOLUBILITY IN WATER, ETC.
(U. s. P. vni.)
loo gms. water dissolve 17.5 gms. salt at 25°.
100 gms. alcohol dissolve 3.08 gms. salt at 25°, and 11.5 gms. at 60°.
100 gms. chloroform dissolve 0.16 gm. salt at 25°.
HYDRASTINE C21H2iNO6. HYDRASTININE HYDROCHLORIDE
CiiHnNO2.HCl.
SOLUBILITY IN SEVERAL SOLVENTS.
(U. S. P. VIII; at i8°-22°, Miiller, 1903.)
Gms. C2iH21NO« per 100 Gms. Gms. per 100 Gms. Solution
Solvent. _ Solution. _ Solvent. at i8°-22°.
' At i8°-22°. At 80°. ' Q1H21NOI^C11H11N02.HC1.
Water 0.033 0.025 Ether 0.51 0.078(25°)
Alcohol 0.74(25°) 5.9(60°) Ether+H2O o.8o
Benzene 8.89 ... Chloroform loo-f- 0.35 (25°)
Ethyl Acetate 4.05 ... CCU 0.123 ...
Petroleum Ether 0.073
HYDRAZIDES 312
HYDRAZIDES.
SOLUBILITY OF THE TAUTOMERIC FORMS OF HYDRAZIDES IN BENZENE AT 5°.
Determined by the freezing-point method. See also p. 487. (Sidgwick, 1915.)
Cms. Compound
Compound. Formula. Dissolved per
Liter Benzene.
form 5.5
Phthalylphenylhydrazide Ce^ <? ^ > N.NH.C6H5 ! •„***
^ CO ' ) C form
i.i
/C0\
Phthalylphenylmethylhydrazide Ce^ \ CQ / N.N(CH3)C6H6, A form 124
HYDRAZINE NH2.NH2.
DISTRIBUTION OF HYDRAZINE BETWEEN WATER AND BENZENE.
(Georgievics, 1915.)
Cms. NH2.NH2 per: Gms. NH.NH, per:
25 cc. H2O Layer. 75 cc. C6H6 Layer. 25 cc. H2O Layer. 75 cc. C6H6 Layer.
0.4137 O.O27 1.7601 0.0626
0.6676 0.0335 2.3336 o.noi
1.0862 0.0355 4-75 0-J37
HYDRAZINE PerCHLORATE N2H4(HC1O4)2.3H2O.
SOLUBILITY IN WATER. (Carlson, 1910.)
,o Sp. Gr. Gms. N2H4(HC1O4)2
Sat. Sol. per 100 cc. Sat. SoL
18 1.264 41-72
35 I-3QI 66.9
HYDRAZINE MonoNITRATE N2H4.HNO3.
SOLUBILITY IN WATER. (Sommer, 1914.)
Gms. N2H4HNp3 per 100 Gms. Gms. N2H4.HNp3 per 100 Gms.
' Sat. Sol. Water. Sat. Sol. Water.
10 63.63 174.9 40.02 85.86 607.2
15 68.47 217.2 45-02 88.06 737-6
20.01 72.70 266.3 5°-01 91.18 1034
25.01 76.61 327.5 55.01 93.58 1458
30.01 80.09 402.2 60.02 95.51 2127
35.01 83.06 490.3
HYDRAZINE SULFATE N2H4.H2SO4.
loo grams water dissolve 3.055 gms. N2H4.H2SO4 at 22°. (Curtius and Jay, 1889.)
Phenyl HYDRAZINE and other substituted hydrazines. See page 486.
HYDRIODIC ACID HI.
SOLUBILITY IN WATER, DETERMINED BY FREEZING-POINT METHOD.
(Pickering, i893a.)
Gm. HI Gms. HI
t°. per 100 Gms. Solid Phase. t°. per 100 Gms. Solid Phase.
Sat. Sol. Sat. Sol.
— IO 20.3 Ice —60 52.6 HI.4H2O
-20 29.3 " -40 59
-30 35.1 « about-35.5m.pt. 64
-40 39 « -40 65.5
— 50 42 " —49 66.3 +HI.3H2O
— 60 44.4 " —48m.pt. 70.3 Hi.3H2o
-70 46.2 " -56 73.5 " +HI.2H20
— 80 47.9 " +HI.4H2O —52 74 HI2H2O
F.-pt. data for HI + H2S (Bagster, 191 1), HI + (CH3)2O. (MaassandMclntosh, 1912.)
HYDROBROMIC ACID
HYDROBROMIO ACID HBr.
SOLUBILITY IN WATER.
(Roozeboom — Z. physik. Chem. 2, 454, '88; Rec. trav. chim. 4, 107, '85; 5. 358, '86; see also Pickering
— Phil. Mag. [5] 36, 119, '93.)
Gms.HBr Dissolved(at 760-765111111.)
per 100 Gms.
Water.
Solution.
255-0
7I-83
239.0
70.50
221 .2
68.85
6II.6
210-3
67.76
581.4
2O4.O
67.10
193.0
65.88
532-1
171 .5
63.16
468.6
I50-5
60.08
406.7
130.0
56.52
344-6
Gms. HBr Dissolved at
Lower Pressures per 100
Gms. H2O.
175.0 (10 mm.)
- 2.5
-15
o
+ 10 210.3 67.76 581.4 108 . 5 (5 mm.)
15
25
50
75
100
For 0 see ethane, p. 285.
F.-pt. data for HBr + H2S (Bagster, 1911); HBr + (CH3)2O, HBr + CH3OH,
HBr + CzHsOH, HBr + CH3COOC2H6 and HBr + C6H6CH3.
(Maass and Mclntosh, 1912.) (Reid and Mclntosh, 1916.)
HYDROCHLORIC ACID HC1.
SOLUBILITY IN WATER BY THE FREEZING-POINT METHOD.
(Composite curve from results of Roloff, 1895; Pickering, 1893 (a); Roozeboom,
1884, 1889 and Rupert, 1909.)
Gms. HC1
t°. per loo Gms
Solid Phase. t°.
Gms. HC1
per loo Gms. Solid Phase.
Sat
Sol.
Sat. Sol.
— I . 706
I
.66
Ice
—
18
•4
48.6
HC1.2H,O
-14.97
10
.02
"
—
17
.7m.
Pt.
50.3
"
-28.84
14
•5i
•
—
18
•7
52.85
"
-40
17
.40
"
—
19
•4
54-i
M
-60
21
•30
"
—
20
.8
55-7
«
-80
24
.20
"
—
21
• 3
56.5
«
-86Eutec.
24
.8
" +HC1.3H20 —
23
.2
57-3
«
— 50
30
.1
HC1.3H20
—
23
-5Eutec.
"
+HC1.H20
-40
32
•7
M
—
21
•5
58^2
HC1.H,O
-30
36
•5
«
—
20
•7
59.1
•
— 24.9m.pt.
40
•3
"
—
18
•4
61.1
"
-27-5
44
" +HC1
.aH2O
—
17
•4
62.4
"
-23.8
45
•7
HC1.2H20 —
15
-4
65-4
'«
— 21.2
45
•9
"
—
15
•35
66.8
"
At about —15.35
two liquid layers are formed. Data for these are
as follows:
HC1 layer.
H2O
layer.
t°of
Saturation
Gms. H2O Gms. HC1
per 100 Gms. t°. per 100 Gms.
Sat. Sol. Sat. Sol.
d. of Sat. Sol. t°.
Gms. HC1
per 100 Gms.
Sat. Sol.
d. of Sat. Sol.
Below —50
O
.008
— 2O
67.
65
• 279
IS
64
70
.231
" -50
o
.017
~~I5
67.
29
.269
20
64
19
.228
Bet. -15 and o°
o
.077
— 10
66.
.260
30
63.21
.229
Above 45
0
.021
-5
66.
44
• 255
35
62
00
.227
"
0
.052
0
65-
85
.247
40
62
27
.218
"
0
.11
+5
65-
48
.245
45
61.76
.212
"
0
•13
10
65-
18
.240
So
61
65
.2IQ
For additional data on this system see Baume and Tykociner, 1914.
HYDROCHLORIC ACID 314
HYDROCHLORIC ACID HC1.
SOLUBILITY IN WATER AT DIFFERENT TEMPERATURES AND
PRESSURES.
o
8
12
14
18
23
30
40
f
60
ioscoe and Dittmar — Liebig's Ann. 112, 334, '59; betow o°, Roozeboom- — Rec. trav.
chim. 3, 104, '84.)
At Different Temperatures and 760 mm. Pressure. At Different Pressures and o°
_A JL —
cc. HClper
ioocc.H2O.
Density. '
^SoF
r Gms. HC1 per
100 g. H2O.
Pressures.*
Gms. HC1 per
100 g. H2O
525-2
1.2257
45 •I5
82.31
60
61-3
497 7
I .2265
44-36
79 73
100
65-7
480.3
1.2185
43 83
78.03
150
68.6
47J-3
I.2I48
43-28
76.30
200
70.7
462 4
1.2074
42.83
74-92
300
73-8
451.2
I . 2064
42-34
73-4i
4OO
76.3
435-o
I.20I4
41 .54
71.03
500
78.2
40.23
67-3
600
80.0
38.68
63-3
750
82.4
. . .
. . .
37-34
59-6
IOOO
85.6
...
35-94
56-1
1300
89-5
* Pressures in mm. Hg minus tension of H2O vapor.
SOLUBILITY IN WATER AT TEMPERATURES BELOW o".
At a pressure of 760 mm. At pressures below and above 760 mm.
t°. q. t°. q. t°. mm. Pressure. q.
-24 IOI.2 -15 93.3 -23.8 ... 84.2
— 21 98.3 —io 89.8 —2i 334 86.8
— 18.3 96 — 5 86.8 —19 580 92.6
— 18 95.7 o 84.2 — 18 900 98.4
-17.7 1073 101.4
For definition of q, see Ethane, p. 285.
The eutectic is at —86° and 33 gms. HC1 per 100 gms. H2O.
SOLUBILITY OF HYDROCHLORIC ACID GAS IN METHYL ALCOHOL, ETHYL
ALCOHOL, AND JN ETHER AT 760 MM. PRESSURE.
(dc Bruya— Rec. tray. chim. u, 129, '92; Schuncke — Z. physik. Chem. 14* 336. *94-)
Grams HC1 gas per 100 Grams Solution in:
CH3OH. C2H6OH. (C2H6)2O.
-10 54-6 ... 37-5I(-9-2°)
- 5
o
+ 5
io
'5
30
25
30
5I-3
45-4
35-6
44.2(6.5°)
42.7(11-5°)
30.35
27 .62
47-o(i8°)
41.0
24.9
40.2 (23.5°)
22.18
43-o(3i.7°)
38-1(32°)
19.47
315 HYDROCHLORIC ACID
SOLUBILITY OF HYDROCHLORIC ACID GAS IN AQ. SULFURIC ACID SOLUTIONS.
(Coppadoro, 1909.)
Results at 17°.
Gms. per 100 Cms.
1 of Sat. Sat. Sol.
Results at 40°.
Gms. per 100 Gms.
d ol Sat. Sat.>l.
Results at 70°.
, , _ Gms. per 100 Gms.
d °cL?at' Sat: S01-
Sol.
H,S04.
HCl. '
oOl.
H2S04.
HCl. '
SoL
H2SO4.-
HCl.'
.211
0
42.7
1.185
3
-56
35-6
1.145
I
.61
32.7
.220
I.
86
39-9
i-i95
5
.86
34-8
1.150
3
-38
3I-I
.220
4-
75
39-2
I. 210
8
.90
32-4
1.160
4
.80
30-5
•235
8.
04
36-9
1-255
16
.80
27.6
1.180
7
•93
28.9
.260
12.
80
33-2
1-255
18
.8
25-9
1.225
18
•9
22.8
•305
2O.
9
28.5
1.340
28
.6
18.5
1.230
20
22-3
•355
30.
8
22.6
I .400
44
.2
"•5
1.315
36
.2
13-2
•430
44-
6
15
1.520
61
.1
3-35
1.380
48
6.99
•545
59-
4
6.26
1-575
66
•4
1.17
1.510
62
•7
1.56
.580
65-
4
3-25
1.650
73
.2
0.17
1.560
67
.6
0-54
i. 660
73-
7
0.62
1-725
79
•4
0.081
1.700
80
•7
0.05
1-735
77-
5
O.II
i-755
81
•4
0.032
1-745
83
0-035
1.815
89
0.068
1.770
83
•5
0.029
1-745
83
-4
0.032
Phenol Rich Layer.
^
% HCl. % Phenol".
o 72
0.09 78
0.2 80 . 3
0.36 82.6
0.52 84.5
% Water.
11.22
84.5
80.38
72.43
60.25
% HCl. % Phenol.
o 88.78
IO.7 4.8
15.64 3.98
24-37 3-2
36-25 3-5
MISCIBILITY OF HYDROCHLORIC ACID WITH MIXTURES OF WATER AND
PHENOL AT 12°.
(Schreinemakers and van der Horn van der Bos, 1912.)
Composition of the Reciprocally Composition of the Solutions in
Saturated Liquid Pairs. Contact with Solid Phenol.
Water Rich Layer.
%HC1. ' % Phenol
o 7-45
3.1 6.6
6.6 5-3
8 5-1
10.7 4.8
Additional data for this system are given by Krug and Cameron, 1900.
FREEZING-POINT DATA (Solubility, see footnote, p. i) FOR MIXTURES OF
HYDROCHLORIC ACID AND OTHER COMPOUNDS.
Hydrochloric Acid + Hydrogen Sulfide (Baume and Georgitses. 1912, 1914.)
11 i A/Toi-t,,,! Al~~t,~| f (Baume and Borowski, 1914; Baume and Pamfil,
- Methyl Alcohol { igil I9u; Maass and Mclntosh, 1913-)
+ Methyl Chloride (Baume and Tykociner, 1914.)
+ Methyl Ether (Maass and Mclntosh, 1912; Baume, 1911, 19x4.)
+ Propionic Acid (Baume and Georgitses, 1912, 1914.)
-j- Sulfur Dioxide (Baume and Pamfil, 1911, 1914.)
HYDROCYANIC ACID HCN.
DISTRIBUTION BETWEEN WATER AND BENZENE.
(Hantzsch and Sebalt, 1899; Hantzsch and Vagt, 1901.)
t. Mol. HCN per Liter; c Mol. HCN per Liter: c
H2O Layer (c). CeH6 Layer (c'). 7'' ' H2O Layer (c) . CgR* Layer (cO-~ ?'
6 0.00625 0.00325 1.923 7 0.0574 0.0148 3.88
16 0.00593 0.00363 1-634 20 0.0572 0.0154 3.72
25 0.00580 0.00375 1.547
Data for the effect of HCl and of KC1 on the distribution are also given.
HYDROFLUORIC ACID HF.
100 grams H2O dissolve in grams HF at —35°. (Metzner. 1894.)
HYDROGEN 316
HYDROGEN H. SOLUBILITY IN WATER.
(Winkler — Ber. 24, 99, 'gx; Bohr and Bock — Wied. Ann. 44, 318, '91; Timofejew — Z. physik.
Chem. 6, 147, oo.)
t°. ft'. _ /. _ ft. q.
a 0.0214 ... ... 0.0214 0.000193
5 0.0203 0.0209 — 0.0241 0.0204 0.000184
10 0.0193 0.0204 — 0.0229 0.0195 0.000176
15 0.0185 0.0200 — 0.0217 0.0188 0.000169
20 0.0178 0.0196 - 0.0205 0.0182 0.000162
25 0.0171 0.0193 — 0.0191 0.0175 0.000156
30 0.0163 ... ... 0.0170 0.000147
40 0.0153 ... ... 0.0164 0.000139
50 0.0141 ... ... 0.0161 0.000129
60 0.0129 ... ... 0.0160 0.000119
80 0.0085 ... ... 0.0160 0.000079
100 o.oooo ... ... 0.0160 o.oooooo
I = Ostwald Solubility Expression, see p. 227. For 0', /3, and q, see Ethane, p. 285.
Data for the solubility of hydrogen in water at pressures up to I o atmospheres
are given by Cassuto, 1913.
SOLUBILITY OP HYDROGEN IN AQUEOUS SOLUTIONS OF ACIDS AND
BASES AT 25°.
(Geffcken — Z. physik. Chem. 49, 268, '04.)
_ Solubility of H (/a = Ostwald Expression) in Solutions of;
peter. HCL HN°3' *H2SO4. CHaCOOH. CH2C1COOH. KOH. NaOH.
o.o 0.0193 0.0193 0.0193 0.0193 0.0193 0.0193 0.0193
0.5 0.0186 0.0188 0.0185 0.0192 0.0189 0.0167 0.0165
i.p 0.0179 0.0183 0.0177 0.0191 0.0186 0.0142 0.0139
2.0 0.0168 0.0174 0.0163 0-0188 0.0180 ... 0.0097
3.0 0.0159 0.0167 0.0150 0.0186 ... ... 0-0072
4.0 ... 0.0160 0.0141 0.0186 ,.. ... 0.0055
The above figures for the concentrations of acids and bases were calculated to
grams per liter, and these values with the corresponding 1& values for the solubility
of hydrogen, plotted on cross-section paper. From the resulting curves, the follow-
ing table was read :
Grams Acids
and Bases
per Liter.
0
20
40
00
80
100
150
2OO
250
Solubility of H (/25 =
Ostwald Expression) in Solutions of:
0
0
O
0
O
O
HCL
.0193
.0185
.0179
.0173
.0167
• Ol6o
HNO3.
0.0193
0.0189
0.0186
0.0183
0.0180
0.0179
0.0171
0.0165
0.0160
*H2S04.
0.0193
0.0186
0.0180
0.0174
0.0168
0.0162
0.0148
0.0140
CH3COOH.
0.0193
0-0192
O.Oigi
0.0190
0.0189
0.0189
0.0188
0.0186
0.0184
CH2C1COOH
0.0193
0.0191
O.OI9O
o.o i 88
0.0187
0.0185
0.0182
0.0179
0
0
o
0
KOH.
.0193
.OI72
•0135
NaOH.
0.0193
0.0165
O.OI4O
O.OII7
0.0097
0.0082
0,0058
For Ostwald Solubility Expression /, see p. 227.
THE SOLUBILITY OF HYDROGEN IN CONC. H2SO< AT 20°.
(Christoff, 1906.)
%H2S04 o 35.82 61.62 95.6
4o 0.0208 0.00954 0.00708 0.01097
317
HYDROGEN
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF AMMONIUM
NITRATE AT 20°.
(Knopp — Z. physik. Chem. 48, 103, '04.)
*'
Normality
(per 1000 Gins.'
H20.
Molecular
Concentra-
tion.
Absorption
Coefficient
of Hydrogen.
Density
•A Solutions.
o.oo
O-OO
o.oo
0.0188
1.037
0.1308
0.002352
0.01872
.0027
2.167
0.2765
0.004956
0.01845
.0072
3-378
0.4363
0.007799
0.01823
• OI22
4.823
0.6333
O.OII280
0.01773
.0182
6.773
0.9069
0.016447
0.01744
.0262
/ / v/
"•550
1.6308
0.028525
0-01647
.04652
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF BARIUM
CHLORIDE.
(Braun — Z. physik. Chem. 33, 735, 'oo.)
Gms.BaClu
per 100 Gms.
Solution.
o.oo
3-29
3-6
6-45
7.00
Coefficient of Absorption of Hydrogen at :
5°.
0.0237
0.02II
O.O2O9
0-0196
0.0194
10°.
0-0221
0.0198
0.0197
0.0186
0.0183
15°.
0.0206
0.0l85
O.Ol84
0.0173
0.0172
20°.
O.OI9I
0.0172
O.OI7O
0.0161
0.0159
2S°-
0.0175
0-0157
0.0156
0.0147
0.0146
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF CALCIUM CHLOR-
IDE, MAGNESIUM SULPHATE, AND LITHIUM CHLORIDE AT 15°.
(Gordon — Z. physik. Chem. 18, 14, '95.)
Coefficient of Absorption of hydrogen in water at 15° = 0.01883.
In Calcium In Magnesium In Lithium
Chloride.
Sulphate.
Chloride.
Gms.
CaCl2
G.M.
CaCl2
Absorption
Coefficient
Gms.
MgSO4
G.M.
MgSO4
Absorption
Coefficient
Gms.
LiCl
G.M.
LiCl
Absorption
Coefficient
per
too g. Sol
per
. Liter.
of H.
per
100 g. Sol.
per
Liter.
of H.
per
100 g. Sol.
Ltter.
of H.
3-47
0.
32I
0.
01619
4-
97
0-433
O.OI5OI
3-48
0.835
0.01619
6.10
0.
578
0.
01450
10.
19
0.936
0.01159
7-34
1.800
0.01370
"•33
I.
122
0.
01138
23-
76
2.501
0.00499
14.63
3-734
0.0099
17-52
I.
1827
0.
00839
26.34
2.
962
0.
00519
For definition of Coefficient of Absorption, see page 227,
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF POTASSIUM
CARBONATE, CHLORIDE, AND NITRATE AT 15°.
(Gordon.)
In Potassium In Potassium In Potassium
Carbonate. Chloride. Nitrate.
Gms.
K2C03
per
100 g. Sol.
2.82
8.83
16.47
24.13
4I.8l
G.M.
K-jCOa
per
Liter.
0.209
0.690
1.376
2.156
4.352
Absorption
Coefficient
of H.
0.01628
0.01183
0.00761
0.00462
0.00l6o
Gms.
KC1
per
100 g. Sol.
3.83
7.48
12.13
19.21
22.92
G.M.
KC1
per
Liter.
0.526
1.051
1-755
2.909
3-554
Absorption
Coefficient
of H.
0.01667
0.01489
0.01279
O.OIOI2
0.00892
Gms.
KNO3
per
100 g. Sol.
4-73
8.44
16.59
21.46
G. M.
KNO3
Liter.
0.482
0.879
1.820
2.430
Absorption
Coefficient
of H.
0.01683
0.01559
0.01311
O.OIlSo
HYDROGEN
318
SOLUBILITY OP HYDROGEN IN AQUEOUS SOLUTIONS OP POTASSIUM
CHLORIDE AND NITRATE AT 20°.
(Knopp — Z. physik. Chem. 48, 103, '04.)
In Potassium Chloride.
In
Potassium Nitrate.
P>
Normality
(per 1000
g.H20).
Absorption
Coefficient.
Density
of
Solutions.
P-
Normality
(per looo
g.H20).
Absorption &*&?
Coefficient. c . °?
Solutions.
1.089
0.1475
o
.01823
I
.0052
I
.224
0
.1245
0.01835
.0059
2.123
0.2907
0
•01757
I
.OIl8
2
.094
O
.2114
o. 01818
.0113
4.070
0.5687
0
.01661
I
.0243
4
.010
0
.4127
0.01785
.0236
6-375
0.9127
o
•01531
I
•0394
5
•925
0
.6225
0.01743
•0359
7.380
1.0682
0
.01472
I
.0460
7
.742
o
.8293
0.01667
.0477
13.612
2.1222
0
•01255
I
.0875
13
.510
I
•5436
0.01436
.0865
SOLUBILITY OP HYDROGEN IN AQUEOUS SOPIUM CARBONATE AND
SULPHATE SOLUTIONS AT 15°.
(Gordon.)
In Sodium Carbonate.
Gms. NazCOa G.M. Absorption
per loo Gms. Na2CO» Coefficient
Solution. per Liter. of H.
2.15 0.207 0.01639
8.64 0.438 0.01385
11.53 1.218 0.00839
In Sodium Sulphate.
Gms. Na2SO4 G. M. Absorption
per loo Gms. Na2SO4 Coefficient
Solution. per Liter. of H.
4-58 o-335 0.01519
8.42 0.638 0.0154
16.69 I-364 0.00775
SOLUBILITY OP HYDROGEN IN AQUEOUS SOLUTIONS OP SODIUM
CHLORIDE.
(Braun; Gordon.)
Gms.NaCl
per ioo Gms.
Solution
1.25
3-80 .
4.48
6.00
14-78
23.84
Coefficient of Absorption of Hydrogen at:
5°.
0.0218
0.0198
0.0192
0.0184
10°.
O.O2O5
0.0188
0.0182
0.0175
15°.
O.OI9I
0.0176
O.OI7I
O.Ol64
0.0093
0.00595
20°.
0.0177
0.0162
0.0159
0.0153
25°.
0.0162
0.0148
0.0143
0.0138
SOLUBILITY OP HYDROGEN IN AQUEOUS SOLUTIONS OP SODIUM
NITRATE.
In Sodium Nitrate at 20°. In Sodium Nitrate at 15°.
(Knopp.) (Gordon.)
Normality
Absorption
Density
Gms. NaNO3
G.M.
Absorption
p.
(per 1000
Gms. H20).
Coefficient
of H.
of
Solutions.
per TOO Gms.
Solution.
NaNOa
per Liter.
Coefficient
of H.
1.041
0.1236
0.01839
I .0052
5-57
0.679
0.01603
2.192
0.2634
0.01774
I.OI30
ii .16
I-4I3
0.0137
4-405
0.5416
0.01694
1.0282
19.77
2.656
0.01052
6.702
o . 8442
O.OI5I8
I .04411
37-43
5-7II
0.00578
12.637
J-7354
0.0130
I .08667
319 HYDROGEN
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF VARIOUS SALTS AT 15°.
(Steiner, 1894.)
Salt in Aq Bunsen Absorption Coefficient 0 (Xio4) in Aq. Solution of Normality.
Solution.
LiCl
KNO3
KC1
NaNO3
NaCl
iMgS04
|ZnSO4
iNa2SO4
0.
I.
2.
3-
4-
5-
6. 7- 9-
1883
1^74
132^
II2I
040
1883
1^24
1276
IO76
1883
1221
QQ3
810
667
--0
1883
I f)O2
1217
006
820
1883
I4O6
I2OI
984
808
667
^42
1883
140?
line
0^8
780
trio
1883
I478
1144
880
699
573
1883
1451
II2O
856
659
499
... ... ...
1883
1446
III3
852
667
1883
I37O
001
7IO
*-3 / w
yvyj.
/ xv
1883
1338
967
700
508
372
273 206 158
1883
I7AO
6OO
1883
1280
731
|Na2CO3
Cane Sugar
SOLUBILITY OF HYDROGEN IN ALCOHOL. (Timofeiew, 1890; Bunsen-Heurich, 1892.)
Coef. of Absorp- Coef. of Absorp- Coef. of Absorption
t°. tion in 98.8% t°. tion in 7% t°. in Pure Alcohol
' Alcohol. Alcohol. (Bunsen).
o 0.0676 4 0.0749 i 0.06916
6.2 0.0693 18.8 0.0740 5 0.06847
.13.4 0.0705 11.4 0.06765
23.7 0.06633
SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 20° AND 760 MM. PRESSURE.
(Lubarsch, 1889.)
Wt. % Alcohol. Vol. % Absorbed H. Wt. % Alcohol. '.Vol. % Absorbed H.
o 1.93 28.57 1.04
9-09 i-43 33-33 i-i7
16.67 I-29 50 2.02
23.08 I.I7 66.67 2.55
SOLUBILITY OF HYDROGEN IN AQ. SOLUTIONS OF CHLORAL HYDRATE.
(Miiller, C. 1912-13.)
Cms. Chloral Absorption Coefficient.
j.o Hydrate per d^ of Aq. , * \
100 Gms. Aq. Solution. ft. fto.
Sol.
19.4 15-5 1.0722 0.01732 0.01724
17.4 28.3 I.I43 0.01569 0.01540
18.7 46.56 1.2505 0.01388 0.01375
16.5 52 1.2870 0.01314 O.OI28O
17 63 I-37I 0.01270 0.01243
17.9 68 1.4097 0.01286 0.01270
18.3 78.4 1-4993 0.01398 0.01380
SOLUBILITY OF HYDROGEN IN CHLORAL HYDRATE SOLUTIONS AT 20°. (Knopp, 1904.)
A Normality (per Molecular Absorption Density
1000 Gms. H2O). Concentration. Coefficient of H. of Solutions.
4.91 0.310 0.005594 0.01839 1.0202
7.69 0.504 0.008992 0.01802 1.0320
14.56 I.O3O O.OI8223 O.OI7I2 1.0669
29.50 2.530 0.043601 0.01542 I.I466
38.42 3-770 0.063647 0.01440 1.1982
49-79 6 0.097493 0.01353 1.2724
63.90 10.700 o. 161660 0.01307 1.3743
For definition of Bunsen Absorption Coef., see p. 227.
HYDROGEN
320
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF GLYCEROL.
Results at 14° and 21°. (Henkel, 1905, 1912.) Results at 25°. (Drucker and Moles, 1910.)
Wt. %
Absorp. Coef.
t .
Glycerol.
0 (See p. 227-)
14
O
0.0193
M
2.29
0.0189
u
5-32
0.0186
u
8-57
0.0182
ft
10.83
0.01815
u
15-31
0.01765
21
0
0.0184
«
2.29
0.0181
It
5.68
0.0177
11
6.46
0.0176
11
10.40
0.0171
u
18.20
0.0160
Wt. %
Glycerol.
% Sat. Sol.
/zs (Ostwald
Expression) .
0
I
0.0196
4
I.OIOI
0.0186
10.5
1.0260
O.OI78
22
1.0542
0.0154
49-8
1.1290
o . 0099
50-5
1.1300
0.0097
52-6
1-1365
o . 0090
67
1.1752
0.0067
80
1.2113
0.0051
82
1.2159
0.0051
88
1.2307
o . 0044
95
1.2502
0.0034
Aqueous Solution of:
. Water alone
Dextrose (Grape Sugar)
Additional data for this system are given by Miiller, C. 1912-13.
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF SEVERAL COMPOUNDS.
(Hiifner, 1906-07.)
Cone, of
Solvent Gms.
per Liter.
O
41-45
87-3
174
60
59
89
75
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF CANE SUGAR AND
OF GRAPE SUGAR. (Mulier, c. 1912-13.)
Urea
Acetamide
Alanine
Glycocol
t.
Absorption Coef. 0.
20. 1 1
O.OlSl
20
20.25
20.28
0.0176
0.0166
0.0152
20.17
20.11
0.0170
0.0180
20.08
20. l6
0.0156
0.0158
Wt. %
Cane
Sugar.
Sp. Gr.
Sat. Sol.
Abs. Coef. to
015-
Wt. %
Grape
Sugar.
Sp. Gr.
Sat. Sol.
Abs. Coef.
5-04
di5 =1
.019
O
.0173
19
3
0
0.0184
14-7
du =i
.060
O
.0151
20
5
12
,2
^20=1
.048
0.0160
20.26
du = i
.084
0
.0146
20
•5
2O
•7
d%Q = I
.084
0.0145
29.86
di3 = i
.128
0
.0126
21
.1
32
•56
^20= I
.130
0.0125
31-74
dn =i
.138
o
.0119
21 ,
,8
45
8
^20=1
.199
O.OIO2
39.65
</i.3.5= i
• 175
0
.0103
21
,2
59
^0=1
.266
0.0078
42.94
^12-5= I
• 195
0
.0094
15-2
ii. 6
12
12.7
ii. 8
13-3
12.6
SOLUBILITY OF HYDROGEN IN AQUEOUS SUGAR SOLUTIONS AT 15°. (Gordon, 1895.)
Gms. Sugar per Gm. Mols. Sugar Absorption
100 Gms. Solution. per Liter. Coefficient of H.
16.67 °-52o 0.01561
30.08 °-993 0.01284
47.65 1.699 0.00892
SOLUBILITY OF HYDROGEN AT 25° (Findlay and Shen, 1912) IN AQ. SOLUTIONS OF:
Dextrin.
Starch.
Gelatin.
<ms. Dextrir
per 100 cc.
1 Sp. Gr.
1*
Gms
per
Starch cn r>~
100 cc. Sp' Gr"
i Gms.
'**• per
Gelatin ,
100 CC.
3-98
1. 012
0
.0194
2
.OI
I
.005
0.0194
I
•53
0.0194
8.58
I.Oig
0
.0191
3
-56
I
.Oil
0.0189
2
.69
0.0189
8.12
1.028
0
.0188
7
•13
i
.024
O.OlSl
4
•74
0.0185
19.20
1.066
0
.0174
9
.29
I
.032
0.0182
5
•7i
0.0182
321
HYDROGEN
SOLUBILITY OF HYDROGEN IN AQUEOUS PROPIONIC ACID SOLUTIONS.
(Braun, 1900.)
Cms. QHsCOOH
per 100 Cms.
Solution.
2.63
3-37
5-27
6.50
9.91
Coefficient of Absorption of Hydrogen at:
5°.
10°.
15°.
20°.
25°.
O. 02 245
O.O2I4
0.0200
0.0188
0.0172
0.0222
0.0212
0.0199
0.0187
O.OI7I
O.O224
O.O2I2
0.0198
O.Ol84
O.OI7I
0.0218
o . 0209
0.0193
0.0183
0.0169
0.0213
o . 0203
O.OI9I
0.0178
0.0160
SOLUBILITY OF HYDROGEN IN RUSSIAN PETROLEUM.
(Gniewasz and Walfisz, 1887.)
Coefficient of absorption (see p. 227) at 20° = 0.0582, at 10° = 0.0652.
SOLUBILITY OF
Results in terms of
Solvent.
Water
Aniline
Amyl Alcohol
Nitrobenzene
Carbon Bisulfide
Acetic Acid
Benzene
Acetone
HYDROGEN IN WATER AND IN ORGANIC SOLVENTS.
the Ostwald Expression, see p. 227. (Just, 1901.)
Solvent. /25- ly\.
Amyl Acetate 0.0774 0.0743
Xylene 0.0819 0.0783
Ethyl Acetate 0.0852 0.0788
Toluene 0.0874 0.0838
Ethyl Alcohol (98 .8 %) o . 0894 o . 0862
Methyl Alcohol 0.0945 0.0902
Isobutyl Alcohol 0.0976 0.0929
fa.
0.0199
0.0285
0.0301
0.0371
0.0375
0.0633
0.0756
0.0764
fc.
0.02OO
0.0303
0.0353
0.0353
0.0336
0.0617
O.O7O7
0.0703
SOLUBILITY OF HYDROGEN IN ETHYL ETHER.
(Christoff, 1912.)
Results in terms of the Ostwald Solubility Expression I (see p. 227).
k = 0.1115, h = 0.1150, /io = 0.1195, As = 0.1259.
Data tor the solubility of hydrogen in metals are given by Sieverts and co-
workers, 1909, 1910, 1912.
HYDROGEN PEROXIDE H2O2.
DISTRIBUTION OF HYDROGEN PEROXIDE BETWEEN WATER AND AMYL ALCOHOL
AT O° AND AT 25°.
(Calvert, 1901; Joyner, 1912.)
Results at O°. (Calvert, Joyner.)
Mok. HA per Liter. jp
A
6.76
6.66
6.63
6 . 66
6.71
Results at 25°.
Mols. H2O2 per Liter.
(Calvert.)
H2O layer (fl
0.146
0.200
0.407
0-749
1.970
Alcohol Layer (A).
0.0216
0.030
0.061
0.113
0.293
H2O Layer (JF). Alcohol Layer (4).
0.094 0.013
0.194 0.028
0.297 0.042
o . 670 o . 095
0.913 0.130
7.01
6.91
7.08
7.09
7.01
Data are also given for the distribution of hydrogen peroxide between aqueous
sodium hydroxide solutions and amyl alcohol at o° and at 25°.
HYDROGEN PEROXIDE
322
DISTRIBUTION OF HYDROGEN PEROXIDE BETWEEN WATER AND ORGANIC SOLVENTS.
(Walton and Lewis, 1916.)
Different amounts of perhydrol (30% H2O2 solution) were added to various
mixtures of water and organic solvents and, after constant agitation for about
i hour, the H2O2 in each layer was determined.
Solvent
Ethyl Acetate
Isobutyl Alcohol
Amyl Acetate
Acetophenone
Ether
Ether
Aniline
t°.
25
25
25
25
25
0
25
Ratio,
Cone. aq.
Solvent.
Methyl Iodide
m Toluidine
Phenol
Quinoline
it
u
t°.
25
25
25
0
25
40
Ratio,
Cone. aq.
Cone. org. solvent
3.92- 4.II
2.58- 2.63
13 "13-2
5.82- 6.06
8.28- Q.II
5-72- 5.85
4.08- 4.IO
Cone. org. solvent
Approx. 200
Approx. 5
4-35 -5-55
0.276-0.391
0.365-0.642
0.516-0.602
The following approximate values, determined at room temp., are quoted from
the dissertation of A. Braun, Univ., Wisconsin, 1914.
Ratio, Ratio, Ratio,
Solvent. Cone. aq. Solvent. Conc- aq. Solvent. Cone. aq.
Conc. org. solvent Conc. Org. solvent Conc. Org. solvent
Ethyl Acetate f Ethylisovalerianate ^ Isobutyl Alcohol £
Nitrobenzene ^ Isoamyl Propionate T\ Propyl Formate |
Acetophenone £ Chloroform ^fa Isobutyl Butyrate ^
Amyl Acetate | Benzene jfo Propyl Butyrate ^
The distribution ratio of hydrogen peroxide between water and ether at 17.5°
varies with concentration from 13.9 to 17.4. (Osipoff and Popoff, 1903.)
HYDROGEN SELENIDE H2Se
SOLUBILITY IN WATER.
(de Forcrand and Fonzes-Diacon, 1902.)
4° 9-65
3-77
Vol. H2Se (at o° and 760 mm.) dissolved
per i vol. H2O
13-2
3-45
22.5
2.70
HYDROGEN SULFIDE H2S.
SOLUBILITY IN WATER.
(Winkler, 1906, 1912.)
t°. Abs. Coef. 0. q.
o 4.621 0.699
5 3-935 0.593
10 3.362 0.505
15 2.913 0.436
20 2.554 0.380
SOLUBILITY IN WATER AND IN ALCOHOL AT t° AND 760 MM. PRESSURE.
(Bunsen and Carius; Fauser, 1888.)
In Water. In Alcohol.
t°.
Abs. Coef. /9
'. q.
t°. Abs. Coef. 0. q.
25
2.257
0-334
60
1.176
0.146
30
2.014
0.295
70
1. 010
0.109
35
1.811
0.262
80
0.906
0.076
40
1.642
0.233
90
0.835
0.041
So
1.376
0.186
100
0.800
0
t°.
i Vol. H20 Absorbs.
0.
Q-
i Vol. Alcohol Absorbs.
o
4- 37 Vols.
H2S (at o° and 760 mm.)
4-
686
0.
710
17.89
Vols. H2S (at o° and 760 mm.)
5
3-97
"
4-
063
0.
615
14.78
«
IO
3-59
«
3-
520
0.
530
11.99
M
15
3-23
"
3-
056
0.
458
9-54
««
20
2.91
«
2.
672
0.
398
7.42
M
25
2.61
"
.
5-96
(24°)
M
30
2-33
«
m
f
t
35
2.08
«
m
40
1.86
«
For /3 and q
The PT and
see Ethane, page 285.
the Px curves for the system H2S + H2O are given
by Scheffer,
1911.
323
HYDROGEN SULFIDE
SOLUBILITY OF HYDROGEN SULFIDE IN AQUEOUS SOLUTIONS OF HYDRIODIC
ACID AT 25° AND 760 MM. TOTAL PRESSURE.
(Pollitzer, 1909.)
Cms, per Liter.
HI. HJST
Mols.
per Liter.
Gms. per Liter.
Mols. per Liter.
'IH'].
[HI].
[H2S].
HI.
H2S.
IH'].
[HI].
[H2S]:
O.2O
O
o.
1040
O
3-54
4.71
4
-38
O.
163
1.23
I
.01
0.
III
129.2
3-78
5-33
5
.005
0.
165
1.74
1
•51
0.
113
193.2
3-85
6.06
5
-695
O.
181
2.18
I
•93
0.
125
246.9
4.26
7-33
6
•935
O.
197
2.Q2
2
.64
0.
138
337-8
4.70
.9-75
9
.21
O.
267
3-71
3
.42
0.142
437-5
4.84
560.4
640.3
728.6
887.2
1179
5-55
5-62
6.17
6.71
9.10
Data for the solubility of hydrogen sulfide in liquid sulfur are given by Pela-
bon, 1897.
Freezing-point lowering data for mixtures of H2S and CH3OH and H2S and
(CH3)2O are given by Baume and Perrot, 1911, 1914.
SOLUBILITY OF HYDROGEN SULFIDE IN AQUEOUS SALT SOLUTIONS AT 25°.
(McLauchlan, 1903.)
NOTE. — The original results are given in terms of •=- which is the iodine titer (I)
of the H2S dissolved in the salt solution, divided by the titer (/o), of the H2S dis-
solved in pure water. These figures were multiplied by 2.61 (see 25° result in
last table on page 322) and the products recorded in the following table as
volumes of H2S absorbed by i vol. of aqueous solution.
Solution.
wNH4Br
iw(NH4)2S04
«NH4C2H3O2
n (NH2)2CO
Grams Salt
I Vols. H2S
per Liter.
k Per
i Vol. Sol.
98
I
2.61
53-4
0.96
2.40
80
0.99
2.58
33
0.82
2.14
16.5
0.91
2.37
77.1
1.09
2.84
60. i
I. O2
2.66
18.22
0-975
2-54
24-52
0.905
2.36
150
0.944
2.46
45°
0.858
2.24
1000
0.863
2.26
Solution.
wKBr
wKCl
wKI
wNaBr
wNaCl
n
SnCAOe
Pure C3H5(OH)3 1000
Similar data are also given for the solubility of H2S in aq. C2H6OH solutions
and in aq. CH3COOH solutions at 25°.
Gms. Salt"
i
Vols. H,S
per Liter.
£' per i Vol. Sol.
119
O
•945
2.47
74-5
0
•853
2.22
IOI
0
•913
2.38
43-5
0
.78
2.04
21.7
0
•89
2.32
166
0
•98
2.56
103
0
•935
2.44
58-5
0
•847
2.21
29.2
0
•93
2.42
• 85
o
•893
2.32
* 35-5
0
•73
1.90
i 17-8
0
•855
2.23
HYDROQUINOL (Hydroquinone) C6H4(OH)2 p.
100 gms. sat. solution in water contain 6.7 gms. hydroquinol at 20°, Sp. Gr. of
sol. = 1. 012. (Vaubel, 1899.)
100 gms. 95%Jormic acid dissolve 6.07 gms. hydroquinol at 20.2°. (Aschan, 1313.)
HYDROQUINOL 324
SOLUBILITY OF HYDROQUINOL IN SULFUR DIOXIDE IN THE CRITICAL VICINITY.
(Centnerswer and Teletow, 1903.)
Determinations made by the Synthetic Method, for which see Note, p. 16.
-0 Cms. Hydroquinol *<> Gms. Hydroquinol j.0 Gms. Hydroquinol
per 100 Gms. SO2 per 100 Gms. SO2 per 100 Gms. SO2
63 0.89 II7.6 4.46 136.7 10.31
73.5 1.22 123.3 5.66 I4I.4 13-3
89.2 2.l8 134.2 8.31 145 14.9
DISTRIBUTION OF HYDROQUINOL BETWEEN WATER AND ETHER AT 15°.
(Pinnow, 1911.)
Cone.* Hydroquinol in: Cone. Hydroquinol in:
H2O Layer. Ether Layer. H2O Layer. Ether Layer.
0.00502 o.oin 0.0502 0.1275
0.01196 0.0249 0.0818 0.2343
0.0128 0.0274 0.1105 °-3543
0.0236 0.0552 0.1411 0.5300
0.0455 0.1148 0.1502 0.5604
* The terms in which the cone, is expressed are not stated.
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES:
Hydroquinol and Naphthalene. (Kremann and Janetzky, 1912.)
1 Pyrocatechol. Qaeger, 1907.)
" Resorcinol.
" £Toluidine. (Philip and Smith, 1905.)
Monochlorohydroquinol and Monobromohydroquinol. (Kuster.iSgi.)
Diacetylmonochlorohydroquinol and Diacetylmonobromohydroquinol.
(Kuster, 1911.)
HYDROXYLAMINE NH2(OH).
HYDROXYLAMINE HYDROCHLORIDE NH2(OH).HC1.
SOLUBILITY OF EACH IN SEVERAL SOLVENTS.
(de Bruyn, 1892.)
Gms. NH2OH Gms. NH2(OH).HC
Solvent. t°. per too Gms. t°. per too Gms.
Solution. Solvent.
Methyl Alcohol (abs.) 5 35 iQ-75 16.4
Ethyl Alcohol (abs.) 15 15 19.75 4.43
Ether (dry) (b. pt.) 1.2
Ethyl Acetate (b. pt.) 1.6
For densities of NH2(OH).HC1 solutions, see Schiff and Monsacchi, 1896.
PhthalylHYDROXYLAMINE C6H4<CO > O.
One liter benzene dissolves 0.33 gm. of the A form of melting point 22O°-226°.
(Sidgwick, 1915.)
HYOSCYAMINE Ci7H23N03.
SOLUBILITY IN SEVERAL SOLVENTS AT i8°-22°.
(Muller, 1903.)
Gms. C17H21NO, Gms. C17H21NO,
Solvent. per 100 Gms. Solvent. per 100 Gms.
Solution. Solution.
Water 0.355 Chloroform 100+
Ether 2 . 02 Acetic Ether 4 . 903
Ether sat. with H2O 3 . 913 Petroleum Ether o . 098
Water sat. with Ether 3.125 Carbon Tetrachloride o . 059
Benzene o . 769
325
HYOSCINE
HYOSCINE (Scopolamine) HYDROBROMIDE, etc.
SOLUBILITY IN SEVERAL SOLVENTS AT 25°. (U. S. P. VIII.)
Grams per too Grams Solvent.
Solvent. Hyoscine
Hydrobromide
C17H21NO4HBr.3H2O.
Water 66.6
Alcohol 6 . 2
Ether
Chloroform o . 133
Hyoscyamine
Hydrobromide
CnHzsNOa.HBr.
very soluble
50
0.062
40
Hyoscyamine
Sulfate
(C17H23N03)2.H2S04
very soluble
15.6
0.04
0.043
Nitro INDAN Carboxylic Acids.
Freezing-point lowering data for mixtures of / nitroindan-2-carboxylic acid
and d nitroindan-2-carboxylic acid are given by Mills, Parker and Prowse, 1914.
CO
INDIGO (C6H4<NH>C:)2.
100 gms. 95% formic acid dissolve 0.14 gm. indigo at 19.8°. (Aschan, 1913.)
INDIUM IODATE In(IO,)8.
IOO gms. H2O dissolve 0.067 gm- In(IO3)3 at 2O°. (Mathers and Schluederberg, 1908.)
IsoINOSITOL C6Hi2O6.
loo gms. H2O dissolve25.i2 gms. C6Hi2O2at i8°and43.22 gms. at 100°. (Muller, 1912.)
IODIC ACID HIO3.
SOLUBILITY OF IODIC ACID IN WATER. (Groschuff, 1906.)
- 0.3
1.69
Ice
16 71.7
mos
— 1. 01
6.81
it
40 73-7
«
- 2.38
26.22
«
60 75.9
H
- 4.72
51.42
«
80 78.3
U
- 6.32
57-6i
K
85 78.7
u
— 12.25
67.40
"
101 80.8
«
-14
69.10
" +HI03
no 82.1
HI03+HI308
-J5
70
(unstable) Ice
125 82.7
HI308
-19
72
« «,
140 83.8
"
0
70.3
HI03
160 85.9
u
SOLUBILITY OF IODIC ACID IN NITRIC ACID. (Groschuff.)
Gms,
. HIO3 per 100 Gms.
*"• ' Aq. 27.73 %HN03 40.88% HNQ,'
Solution. Solution. Solution.
0
74.1
18 9
20
75-8
21 10
40
77-7
27 14
60
80
38 18
IODINE I2
SOLUBILITY OF IODINE IN WATER. (Hartley, 1908.)
j.o Gms. I per 1000 Gms.
H20.
18 0.2765
25 0-3395
35 0.4661
45 0.6474
55 0.9222
The above determinations were made with great care. Results for single
temperatures in good agreement with the above are given by Dietz, 1898;
Jakowkin, 1895; Noyes and Seidensticker, 1898; Sammet, 1905; Bray and
Connolly, 1910, 1911; Herz and Paul, 1914 and Fedotieff, 1911-12.
IODINE
326
SOLUBILITY OF IODINE IN AQUEOUS MERCURIC CHLORIDE AND IN AQUEOUS
CADMIUM IODIDE SOLUTIONS AT 25°.
In Aq. HgCl2.
(Herz and Paul, 1914.)
Gms. per Liter.
Millimols per Liter.
o
94-44
124.42
iQS-42
334-6o
1-3.4
12.94
14.60
18.06
25-43
HgCl2.
o
25.64
33-78
54-29
90.84
I.
0.340
3-285
3.706
4-583
6.454
In Aq. CdI2.
(Van Name and Brown, 1917.)
Gms. per Liter.
CdI2.
3-66
45.78
91.56
183.12
I.
2.072
9.056
11.386
14.040
SOLUBILITY OF IODINE IN VERY DILUTE AQUEOUS SOLUTIONS OF POTASSIUM
IODIDE.
(Determinations made with very great care.)
Results at o°.
Results at 25°.
Results
at 25°.
(Jones and Hartman, igiS-)
(Bray and MacKay, 1910.) (Noyesand Seidenstricker, 1898.)
Normality A
Gms. I per
Normality
Millimols I2
Normality
Millimols I2
KIAs2i. Sallol.
ioo Gms.
Sat. Sol.
of Aq.
KISol.
per Liter j
Sat.Sol.
of Aq.
KISol.
per Liter
Sat. Sol.~
O.OOO992
.OOO2
0.0282
0
1-333
O
1.342
O.OO2OO
.OOO4
0.0409
0.001
1.788
0.00083
1.814
0.00500
.OOIO
o . 0760
O.OO2
2.266
0.00166
2-235
O.OIOOO
.OO2O
0.1356
0.005
3.728
0.00664
4.667
0.01988
.0044
0-2533
O.OIO
6.185
0.01329
8.003
O.O500 3
.OIO9
0.609
O.O2O
11.13
0.02657
4.68
0.09993
.O2I9
1.199
0.050
25-77
0.05315
28.03
0.100
51-35
0.1063
55-28
SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF POTASSIUM IODIDE AT
25° AND VICE VERSA.
(Parsons and Whittemore, 1911.)
(Time of rotation 6 mos. or longer. Duplicate determinations at different lengths of time, were made.)
Solid
Sp. Gr.
Sat. Sol.
Gms. per ioo Gms.
Sat. Sol.
KI I
1-349
16.03 18.49
1.516
19.70 26.16
1.769
22.88 36.06
1.910
23.55 40.52
2.403
24.78 53.60
2.904
25 63.12
3.082
25.18 66.04
3-3*6
26 68.09
Solid
Sp. Gr.
Gms. per ioo Gms.
Sat. Sol.
Phase.
Sat. Sol.
KI I
dine
3-246
27.92 66.45
29.71 62.81
2.665
35.80 49.61
2-539
38.09 44.58
2.216
44.82 31.01
2.066
49.04 23.08
1.888
54.41 11.63
+KI
1-733
60.39 o
KI
Additional data for this system are given by Bruner, 1898; Hamberger, 1906;
and Lami, 1908.
Data for the solubility of iodine in aq. 40% ethyl alcohol and aq. 60% ethyl
alcohol solutions of potassium iodide at 25°, are given by Parsons and Corliss,
1910. The solid phases were identified in each case and it was demonstrated
that no polyiodides of potassium exist in the solid phase or in solution at 25°.
An extensive series of determinations of the simultaneous solubility of iodine
and potassium iodide in nitrobenzene and in other organic solvents, as well as
in mixtures of nitrobenzene and other solvents are given by Dawson and Gawler,
1902, and Dawson, 1904. The determinations were made to obtain information
on the formation of polyiodides in solution. The molecular ratio of dissolved
I2/KI was found to be I or more in all cases. (See also p. 537.)
Freezing-point lowering data, determined by time-cooling curves, for mixtures
of iodine and potassium iodide are given by Kremann and Schoulz, 1912. Data
for this system are also given by Olivari (1908).
327 IODINE
SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF POTASSIUM BROMIDE
AND OF SODIUM BROMIDE AT 25°.
(Bell and Buckley, 1912.)
In Aq. KBr
Solutions.
In Aq. NaBr
Solutions.
Cms. KBr
Gm. Atoms I
Gms. NaBr
Gm. Atoms I
per Liter.
per Liter.
per Liter.
per Liter.
60.6 ty
0.0176
2,^ 96.4
0.0266
106.9
0.0278
I87.7
0.0425
175-9
0.0415
271.8
0.0538
229.8
0.0532
357-4
0.0598
281.9
0.0628
422.21
0.0638
33° -6
0.0717
499.1 •
o . 0648
377-1
0.0797
569-9
o . 0644
411
0.0864
632
0.0622
461.7
o . 0948
679.7
0-0595
509.8
0.1006
750-5
0.0551
567.9 sat.
0.1094
756.1 sat.
0.0550
SOLUBILITY
OF IODINE IN
AQUEOUS SOLUTIONS OF ACIDS.
Aqueous Acid.
Mols. I per Liter Gms. I per Liter
Sat. Sol. Sat. Sol.
Authority.
o.ooi wHCl
0.001332
° • 338 (Bray and MacKay, 1910.)
o.iorcHNOs
0.001340
0 . 340 (Sammet, 1905.)
o . 10 n H2SOi
O.OOI342
0.341
«
SOLUBILITY OF IODINE IN AQUEOUS SODIUM IODIDE SOLUTIONS.
(Gill, 1913-14.) i
Aqueous Nal solutions were prepared by dissolving the stated amounts of the
salt in water and diluting to 100 cc. An excess of iodine was added to each of
these solutions, the mixtures heated to 60° and shaken for several minutes.
They were then allowed to cool in a thermostat at 25° for four hours. The
dissolved iodine in weighed amounts of the saturated solutions was titrated with
thiosulfate. The densities of the Aq. Nal mixtures and also of the solutions
after saturation with iodine were determined.
Gms. Nal &* of d25 of Aq. Nal Gms. I Dissolved
per zoo cc. Aq. Nal after Saturation at 25° per 100 Gms.
Aq. Solution. Solution. with I. of the Sat. Sol.
5 1.0369 1.0698 4.99
10 1.0720 1-1415 9.96
15 1.1072 1.2162 J4-93
20 I.I458 1.2998 20.02
Determinations at other temperatures were made in an apparatus which per-
mitted constant stirring of the solutions at the several temperatures. Results,
interpolated from the original, are as follows:
Gms. I Dissolved per 100 Gms. Gms. I Dissolved per 100 Gms.
0 Sat. Solution in Aq. Nal of: Sat. Solution in Aq. Nal of:
10 Gms. per 20 Gms. per 10 Gms. per 20 Gms. per
100 cc. 100 cc. 100 cc. loo cc.
10 8.9 17.6 30 10.3 20.5
15 9-3 l8-3 40 10.9 22
20 9.6 19 50 11.7 23.4
25 10 19.4 60 12.6 24.9
IODINE
328
SOLUBILITY OF IODINE IN AQUEOUS SALT SOLUTIONS AT 25°.
(McLauchlan, 1903.)
Q,. Gms. Salt
per Liter.
NaaSO4 29.77
KaSO4 43.5
(NH4)2SO4 33
Gms. Dissolved
I per Liter.
0.160
0.238
0.246
. Salt.
NH4C1
NaBr
KBr
Gms. Sak.
per Liter.
53-4
103
119
Gms. Dissolved
I per Liter.
0-735
3-29
3.801
NaNO3
85
0.257
NHjBr
98
4.003
KN03
IOI.2
0.266
NH4C2HsO2
77-i
0.440
NHiNOs
80
0-375
(NH4)2C204
86.9
0.980
NaCl
S8.5
0-575
HaBOs
55-8
0.300
KC1
73-6
0.658
SOLUBILITY OF IODINE IN NITROBENZENE SOLUTIONS CONTAINING VARIOUS
IODIDES AT ROOM TEMPERATURE. SOLUTIONS SAT. WITH I IN EACH CASE.
(Dawson and Goodson, 1904.)
Iodide.
Gms. per Liter.
Iodide.
Iodine.
Potassium Iodide
12-35
112.7
« «
45-56
295-7
« «
115.8
698.2
« «
155-2
943-6
Sodium Iodide
13-55
125
« «
57-7
393
« a
log: I
738
« «
228
1251
Rubidium Iodide
85.4
421
Rubidium Iodide
217-5
1060
Lithium Iodide
84.1
642
Iodide.
Caesium Iodide*
Caesium Iodide
Ammonium Iodide
Ammonium Iodide*
Aniline Hydriodide
Dimethylaniline Hydriodide
Tetramethylammonium Iodide
Tetramethylammonium Iodide
Strontium Iodide
Barium Iodide
Barium Iodide
* Solvent = o nitrotoluene instead of nitrobenzene.
Gms. per Liter.
Iodide.
48.2
223
69.5
94-3
164
160
49-3
51-4
106.5
42.2
158.5
Iodine.
213
858
482
669
721
626
266
280
599
237
809
Similar results are also given for solutions containing KI in addition to the
other iodide, and one series for the simultaneous solubility of KBr and I in nitro-
benzene. It is considered that the increased solubility is most easily explained
on the assumption that periodides are formed in solution.
SOLUBILITY OF IODINE IN AQUEOUS ETHYL AND NORMAL PROPYL ALCOHOL
SOLUTIONS AT 15°.
(Bruner, 1898.)
In Aq. Ethyl Alcohol.
In Aq. (n.) Propyl Alcohol.
Vol. %
C,H5OH
insolvent.
Gms. I per
100 cc.
Solution.
Vol. %
r1 TT f\tr
\*2 iL^Jti.
in Solvent.
Gms. I per
100 CC.
Solution.
Vol. %
CaH7OH
in Solvent.
Gms. I per
100 cc.
Solution.
Vol. %
CSH7OH
in Solvent.
Gms. I per
ICO CC.
Solution.
10
0.05
60
I.I4
IO
0.05
60
2.71
20
0.06
70
2-33
20
O.II
70
4.10
30
0.10
80
4.20
30
0.40
80
6.05
40
0.26
90
7-47
40
o-94
90
9.17
50
0.88
100
15-67
50
1.64
100
14-93
329 IODINE
SOLUBILITY OF IODINE IN AQUEOUS ETHYL ALCOHOL AND IN AQUEOUS ACETIC
ACID SOLUTIONS AT 25°.
(McLauchlan, 1903.)
In Aq. C2H6OH Solutions. In Aq. CH3COOH Solutions.
Gms. I per
ioo cc. Sat.
Gms. CH3COOH
per too Gms.
Gms. I per
ioo cc. Sat.
Solution.
Solvent.
Solution.
0.034
0
0.034
0.039
20 .
0.076
0.172
39-5
0-173
0-955
61.1
0.510
6.698
80.7
I-363
24.548
IOO
3.l62
Cms.
per 100 Gms.
Solvent.
O
4-55
28.48
44.41
72-51
100
SOLUBILITY OF IODINE IN AQUEOUS GLYCEROL SOLUTIONS AT 25°.
(Herz and Knoch, 1905.)
Density of glycerine at 25°/4° = I-2555'» impurities about 1.5%.
Wt.% Glycerine Millimols I Grams I per Density of
inSolvent. per 100 cc. Solution. loocc. Solution. Solutions at 25 °/4°.
o 0.24 0.0304 0.9979
7.15 0.27 O.O342 1.0198
20-44 0.38 0-0482 I.047I
31.55 0-49 0.0621 1.0750
40.95 0.69 0.0875 1.0995
48.7 1.07 0.135 1.1207
69.2 2.20 0.278 LI765
ioo. o 9.70 1-223 1.2646
ioo gms. glycerol (du = 1.256) dissolve 2 gms. iodine at i5°-i6°.
(Ossendowski, 1907.) >
SOLUBILITY OF IODINE IN BENZENE, CHLOROFORM, AND IN ETHER.
(Arctowski — Z. anorg. Chem. n, 276, '95-'96.)
In Benzene. In Chloroform. . In Ether.
t°.
Gms. I per ioo
Gms. Solution.
A o Gms. I per ioo ^ 0 Gms. I per ioo
Gms. Solution. Gms. Solution.
4.7
8.08
-49
0.188 -83 15.39
6.6
8.63
-55*
0.144 —90 14-58
10.5
9.60
-60
0.129 — 108 15-09
10-44
— 69 J
0.089
16^3
11.23
-73i
0.080
+ 10
i . 76 per ioo gms. CHC13
(Duncan — Pharm. J. Trans. 22, 544, 'pi-'
SOLUBILITY OF IODINE IN BROMOFORM, CARBON TETRACHLORIDE, AND IN
CARBON DISULFIDE AT 25°.
(Jakowkin, 1895.)
I liter of saturated solution in CHBr3 contains 189.55 gms. I.
i liter of saturated solution in CC14 contains 30.33 gms. I.
I liter of saturated solution in CSa contains 230 gms. I.
IODINE
330
— 100
- 80
- 63
— 20
— 10
SOLUBILITY OF IODINE IN CARBON BISULFIDE.
(Arctowski, 1894.)
Gms. I per 100
Gms. Solution.
0.32
0.51
1.26
4.14
S-S2
O
10
15
20
Gms. I per 100
Gms. Solution.
7.89
10.51
12-35
14.62
10.92
3°
36
40
42
[Gms. I per 100
Gms. Solution.
19.26
22.67
25.22
26.75
SOLUBILITY OF IODINE IN SEVERAL SOLVENTS AT 25°.
(Herz and Rathmann, 1913.)
Iodine
Solvent.
Chloroform
Carbon Tetrachloride
Tetrachlorethylene
One liter sat. solution of iodine in nitrobenzene contains 50.62 gms. I at i6°-i7°.
(Dawson and Gawler, 1902.)
IOO gms. hexane dissolve 1 .32 gms. iodine at 25°. (Hildebrand, Ellefson and Beebe, 1917.)
100 gms. sat. solution of iodine in anhydrous lanolin (melting point 46°), con-
tain 5.50 gms. iodine at 45°. (Klose, 1907.)
Iodine per Liter of
Sat. Sol.
Solvent.
Trichlorethylene
Tetrachlorethane
Pentachlorethane
Iodine per Liter of
Sat. Sol.
Mols.
0-352
0.237
0.241
Gms.
44.68-
30.08
3° -59
Mols.
0.312
0.244
0.272
Gms.
39.61
30-97
34-53
SOLUBILITY OF IODINE IN MIXTURES OF CHLOROFORM AND ETHER AT 25°.
(Harden and Dover, 1916.) ',
Gms. CHC13 per 100 Gms. Iodine per 100
Gms. CHC13+(C2HB)2O. Gms. ~
O
10
20
30
40
5°
3S-i
29.6
24.8
20.2
I6.3
12.7
Gms. CHC13 per 100 Gms. Iodine per 100 Gms.
Gms. CHC13+(C2H5)2O. CHC13+(C2
60 9.83
80
90
loo
7-5
5-73
4.31
3.10
loo cc. of a mixture of CHC13 + CSa (3:1) dissolve 7.39 gms. iodine (t° ?.)
The addition of S even up to the point of saturation does not affect the amount
of iodine held in solution. (Olivari, 1908.)
Diagrammatic results for mixtures of iodine and each of the following com-
pounds are given by Olivari, 1911: CHI3, p C6H4Br2, [C6H4]N2, p C6H4(NO2)2,
(C6H6CO)2O and C6H6COOH. '
SOLUBILITY OF IODINE IN MIXED SOLVENT
(Stromholm, 1903.)
Gms. I
Solvent. per Liter SoK
Sat. Sol.
Ether 206 . 3 Ether+ 20.96 grr
Carbon Bisulfide 178.5 Ether+4i.9
Ether+3.96 gms. H2O per liter 221 CS2 +22.5
' +7.91 gms. H2O 235.7 CSa +45.1
' +excessH2O 251.4 Ether+47.63
1 +9.79 gms. C2H6OH " 219.1 CS2 +50.06
" +19.6 " " " 231.5 Ether+8o.3
' +294 " " " 243-9 Ether+77.8s
" +39.2 " " « 254.4 CS-j +62.2
S AT 1 6.6°.
ent.
is. CS2 per liter
CS2
ether
ether
CHCU
CHCU
C6H6
CH3I
S
Gins. I
per Liter
Sat. Sol.
202.3
217.2
189.3
201. I
195-2
172.8
204.1
22O.2
189.4
One liter sat. solution in ether contains 167.3 Sms. I at o°. (StrSmholm, 1903.)
331 IODINE
SOLUBILITY OF IODINE IN MIXTURES OF CHLOROFORM AND ETHYL ALCOHOL,
CHLOROFORM AND NORMAL PROPYL ALCOHOL, CHLOROFORM. AND BENZENE,
AND CHLOROFORM AND CARBON DISULFIDE AT 15°.
(Bruner, 1898.)
Vol °f CHCI ^ms' * Dissolved per 100 cc. of Mixtures of:
insolvent. 3
O
10
20
30
40
50
60
70
80
'QO
IOO
SOLUBILITY OF IODINE IN MIXTURES OF CARBON TETRACHLORIDE AND BEN-
ZENE AND IN MIXTURES OF CARBON TETRACHLORIDE AND CARBON DISUL-
FIDE AT I
CHC13+C2H5OH.
CHC13+C3H7OH.
CHC13+C6H6.
CHClj+CSs.
I5-67
14-93
10.40
17.63
9-43
13.16
9.84
15.93
8.69
11.20
8.78
14.20
7.80
8.98
7-74
12. l6
7.09
8.09
6.96
IO.2O
6.62
7.82
6.20
9.08
6.24
7.09
5-34
7.72
5-77
6.42
4.89
6.42
5-06
5-54
4-53
5-27
4-34
4-52
4.07
4.32
3.62
3.62
3.62
3.62
1898.)
Vrti of rr\ Gms. I per 100 cc. of Mixture of: v i o/ rn Gms. I per 100 cc. of Mixture of:
VOl. /Q V^^i4 -^_,^ _Ai - _ VOI. /o l_,l_J4 ji
*» Solvent. ' CCU+CeHe. CCU+CS,. ' in Solvent. 'ca+C^. CCU+CS,/
o 10.40 17.6 60 4.90 5-55
10 9.44 14.44 70 4.09 4.50
20 8.53 12.33 80 3.41 3.37
30 7.77 10.34 90 2.74 2.60
40 6.63 8.60 loo 2.06 2.06
50 5.70 6.83
In the case of the above determinations the volume change occurring on mixing
the solvents was neglected. The temperature was not accurately regulated and
the mixtures not shaken during the saturation. The curves plotted from the
results are not smooth.
DISTRIBUTION OF IODINE BETWEEN WATER AND BROMOFORM^ WATER AND CAR-
BON BISULFIDE, AND WATER AND CARBON TETRACHLORIDE AT 25°.
Qakowkin, 1895.)
The original results were plotted on cross-section paper and the following table made from the curves.
Jakowkin points out that the results of Berthelot and Jungfleisch, 1872, are^incorrect on account of the
presence of HI.
Gms. I per Liter Gms. I per Liter of:
of H2O Layer
in Each Case.
0.05
0.10
0-15
0.20
0.25
A theoretical discussion of the results of Jakowkin is given by Schiikarew (1901).
CHBr3 Layer.
CSj Layer.
CCU Layer.
20
30
4
45
60
8.5
71
91
13
IOO
126
17-5
130
160
22
IODINE
332
DISTRIBUTION OF IODINE BETWEEN CARBON DISULFIDE AND
AQ. POTASSIUM OXALATE.
(Dawson — Z. physik. Chem. 56, 610, '06; Dawson and McRae — J. Chem. Soc. 81, 1086, '02.)
Concentration
flf
Gms. I per Liter of
Aq. K2C204.
Aq. Layer. CS2 Layer.
.0 Equiv.
2.408 10.82
.0 "
3-555 l6-32
.0 "
5.766 27.91
.0 "
6.861 34-01
.2 "
3-525 J7-o7
Vol. of Solution
which Contains
i Mol. I.
Fraction of I
Uncombined
in Solution.
105.3 0.005495
71.37 0.00561
43-99 0.005915
36.98 0.006055
71.97 0.005645
DISTRIBUTION OF IODINE BETWEEN AMYL ALCOHOL AND WATER AND
BETWEEN AMYL ALCOHOL AND AQUEOUS POTASSIUM IODIDE
SOLUTIONS AT 25°.
(Herz and Fischer — Ber. 37, 4752, '04.)
The original results were plotted on cross-section paper, and the
following tables made from the curves.
Millimols I per 10 cc. of H2O and of Aq. KI Layers.
Amyl Alcohol Layer
'
N
2N
3N
4N
ioN
in Each Case.
H-jO.
— K.I.
— KI.
- — KI.
' — K I
• KI.
10
10
10
IO
IO
2-5
O.OI2
0-135
0.160
0.170
0.170
O.OI4
0.150
0.185
O.2OO
O-2OO
0.160
4.0
O.OlS
0.180
0.235
0.255
O.27O
O.24O
5
O.O2I
O.2IO
0.280
0.340
0.315
6
O.025
0.230
0-330
0-375
0.410
0.390
7
O.O29
0.250
0-375
0.430
0.480
0.470
8
. . .
0.26o
0.420
0.490
0-550
o-555
9
0.270
0.450
0-550
O.62O
0-640
10
. . .
0.280
0.470
0.605
0.690
0.720
12
. . .
. . .
0.490
0.700
0.830
0.900
14
0.510
0.790
0.980
1.200
20
...
0-575
Grns.Iperioocc.
Amyl Alcohol Layer
Gms. I per
ioo cc. of H2O and of KI
Layers.
/J
N
aN
N
N
N ""*
in Each Case.
H20.
— KI.
— KI.
— KL
— KI.
— — KI.
10
10
10
10
IO
3
O.OI4
0.164
O.2O
0.21
0.21
4
c 016
0.196
O.24
O.26
O.26
0.21
6
^•026
0.252
o-34
0.38
O.4O
o-37
8
o*-o33
0.297
0.43
0.49
0-54
0.51
10
0.040
0.328
0.51
0.61
0.67
0.69
12
0.341
0.58
o-73
0.81
0.84
14
0.60
0.83
o-95
1. 00
16
0.63
0.91
1.09
1.20
18
0.64
25
0.71
The original figures for sN/io and loN/io KI solutions give prac-
tically identical curves.
Results for the distribution of Iodine between N/io KI solutions on
the one hand, and mixtures in various proportions of C6H64- CS3,
C6H6CH3+CS2, C6H6 + C6H6CH3, C6H6 + ligfft petroleum, CS2 + light
petroleum, CS3+CHC13, CHC13+ CCH6, CC14 + CS2 and CC14+ C6H6CH,
on the other hand, are given by Dawson — J. Chem. Soc., 81, 1086, '02,
333
IODINE
DISTRIBUTION OF IODINE BETWEEN WATER AND IMMISCIBLE ORGANIC SOLVENTS.
Results for Water Results for Water Results for Water Results for Water
-f Carbontetra- + Nitrobenzene + Carbon Disul- + Chloroform
chloride at 18°. at 18°. fide at 15°. at 25°.
(Dawson, 1908.) (Dawson, 1908.) (Dawson, 1902.) (Herz & Kurzer, 1910.)
Mols. Iodine per Liter. Mols. Iodine per Liter. Gins. Iodine per Liter. Mols. Iodine per Liter.
'H2O Layer. CCU Layer.
0.000416 0.0344
0.000535 0.0443
Results for Water
+ Trichlorethyl-
ene at 25°.
(Herz & Rathmann, ' 13.)
Mols. Iodine per Liter.
H2O Layer. CeHsNOz Layer
0.00019 0.0333
o . 00050 o . 0854
0.00133 0.2275
0.00189 0.3328
Results for Water
+ Tetrachlor-
ethylene at 25°.
(Herz & Rathmann,; 13.)
Mols. Iodine per Liter.
.H2O Layer. CSj Layer.
0.0452 27.85
0.0486 30.09
0.0486 30.31
Results for Water
+ Tetrachlor-
ethane at 25°.
(Herz $; Rathmann, '13.)
Mols Iodine per Liter.
H20 Layer. CHC1, Layer."
0.00025 0.0338
0.00120 0.1546
0.00184 0.2318
0.00259 0-3439
Results for Water
+ Pentachlor-
ethane at 25°.
(Herz & Rathmann, '13.)
Mols. Iodine per Liter.
' H2O CHC1.CC12
Layer. Layer.
0.00046 0.0543
O.oooyo 0.0778
O.OOII2 0.1275
0.00236 0.2672
' H20 CC12.CC12
Layer. Layer.
O.OOO88 0.0653
O.OOI27 0.0932
0.00172 0.1285
0.00281 0.2161
• H20 CiH,(V
Layer. Layer.
0.00119 O.lioi
0.00145 0.1247
0.00159 0.1479
0.00217 0.2103
H20 C2HC151
Layer. Layer.
0.00092 0.0848
0.00117 0.1067
0.00160 0.1434
o . 00204 o . 1963
Data for the distribution of iodine between water and mixtures of
at 25° are given by Herz and Kurzer, 1910.
Data for the distribution of iodine between carbon disulfide and aqueous solu-
tions of each of the following iodides at 25° are given by van Name and Brown,
1917. Cadmium iodide, cadmium potassium iodide, lanthanum iodide, nickel
iodide, strontium iodide, zinc iodide and zinc potassium iodide. Results for the
distribution of iodine between carbon tetrachloride and aq. mercuric potassium
iodide are also given.
Results for distribution between CS-5 and aq. BaI2 sols, are given by Herz and
Kurzer, 1910.
Data for the distribution of iodine between carbon disulfide and aqueous solu-
tions of potassium iodide at 15° and at 13.5°, and between carbon disulfide and
aqueous solutions of hydriodic acid at 13.5°, are given by Dawson, 1901 and 1902.
Data for the distribution of iodine between carbon tetrachloride and aqueous
solutions of mercuric bromide and of mercuric chloride at 25° are given by Herz
and Paul, 1914.
DISTRIBUTION OF IODINE BETWEEN CARBON DISULFIDE AND AQ.
t; ETHYL ALCOHOL AT 25°. (Osaka, 1903-08.)
Gms. C2H5OH
Gms. Iodine per Liter:
Gms. CsHfiOH Gms. Iodine per Liter:
per 100 cc.
Aq. Alcohol.
CSz Layer
c.
Aq. Alcohol
Layer c'.
c''
per 100 cc.
Aq. Alcohol.
CSz Layer
c.
Aq. Alcohol
Layer c'.
c'
7.6
O,
,072
35-86
O
.0020
I9.I
0.330
97
o,
0034
7-6
O,
211
107.79
o
.0020
22.9
O.II5
23-78
Q
,0048
ii. 4
o
077
32.93
0
.0023
22.9
0.418
89.61
o
0047
ii.4
o
,280
133.22
0
.0021
26.7
0.0756
9-8
o
.0077
15-3
o
075
25.61
0
.0029
26.7
0-495
65.10
o
.0076
iS-3
o
315
115-34
0
.0027
30.5
o . 0636
4.90
0
.0130
19.1
o
•045
I3-42
0
.0034
30.5
0.546
42.27
o
.0129
DISTRIBUTION OF IODINE BETWEEN ETHER AND ETHYLENE GLYCOL. (Landau, 1910.)
Results at 25°.
Gms. Iodine per Liter:
Results at o°.
Gms. Iodine per Liter:
a
r
.48
.80
.75
.76
•75
.80
(C2H5)20
Layer (c).
2.139
7.820
16.620
20.564
3L785
79-950
(CH2OH)2
Layer (b),
1-449
4-347
9.486 1
11.685
18.135
44.460
(C2H5)20
Layer (a).
(CH2OH),
Layer (b).
r
2.208
1.449
•52
4-255
2.541
.60
7.728
4-347 J
.78
16.200
9.120
.78
30.322
17.062
.78
78.195
44-460 3
.76
IODINE
334
DISTRIBUTION OF IODINE BETWEEN GLYCEROL AND BENZENE AND BETWEEN
GLYCEROL AND CARBON TETRACHLORIDE.
(Landau, 1910.)
Results for Glycerol and Benzene.
Grams Iodine per Liter: /M
Results for Glycerol and CC14.
Gms. Iodine per Liter: /M
t°- Glycerol Layer
(o)
Benzene Layer.
(b) '
to'
t • Glycerol Layer
(a)
CC14 Layer.
(b)
(a)
25°
0.407
I
.922
4
.72
25°
0.365
0
.565 1
•55
ft
0.676
4
.086
6
.04
u
0
.684
I
.224 ]
.78
tt
1.470
10
.212
6
•95
"
I
.416
2
.652 :
.87
n
2.622
20
.102
7
.67
"
5
.064
9
.888 'i
•95
n
5.280
42
.458
8
.04
"
7
.636
14
.766 3
•93
40°
0-459
2
.168
4
.72
40°
o
.322
0
•575
•79
It
0.658
3
.911
5
•94
tl
o
.690
I
.169 1.74
It
1.584
II
.244
7
.10
tl
i
.224
2
.772 1.69
11
3.048
24
.104
7
.91
"
2
.832
6
.444 2.26
11
46
.960
8
•44
"
6
•854
15
.410 2.25
50°
0.467
2
.194
4
.70
So°
0
.299
0
.653 2.19
It
0.642
3
.864
6
.02
It
0
• 570
I
.270 2.23
"
1.463
II
.196
7
•65
"
I
• 5"
3
•457 2.29
tl
2.391
19
.872
8
•31
It
2
.664
6
.468 2.43
"
46
.782
8
.69
It
6
.348
16
.008 2.52
DISTRIBUTION OF IODINE BETWEEN GLYCEROL AND CHLOROFORM.
Results at 25°.
(Herz & Kurzer, 1910.)
Results at 30°.
(Hantzsch & Vagt, 1901.)
Results at Dif. Temps.
(Hantzsch & Vagt, 1901.)
Mols. Iodine per 1000
Gms.
c
Mols. Iodine per Liter:
c
Mols. I per Liter:
C
Glycerol
CHC13
c'
Glycerol
CHC13
c'
Glycerol
CHClj
c'
Layer c.
Layer c'.
Layer c.
Layer c'.
Layer c.
Layer c'.
0.0244
0.0564
O
•43
0.00097
0.00172
0.056
O
0.0119
0.0177
0.675
0.0397
0.0919
0
•43
O.OO2O4
0.00412
0-495
20
0.0084
0.0213
0.400
0.0500
O.II5I
0
•43
0.00418
0.00898
0.465
40
0.0077
O.O22I
0-349
0.00782
0.0216
0.362
50
0.0074
O.O226
0.330
Data are also given by the above named investigators for the distribution of
iodine between aqueous glycerol solutions and chloroform at several temperatures.
DISTRIBUTION OF IODINE BETWEEN GLYCEROL AND ETHYL ETHER.
(Hantzsch & Vagt, 1901.)
Mols. Iodine per Liter:
O
30
30
Glycerol Layer
(c).
0.00566
0.00544
0.00100
Ether Laver
(0-
O.027O
0.0272
O.OO5I
?*
0.21
O.2O
0.20
FREEZING-POINT DATA (Solubility, see footnote, p. I)FOR MIXTURES
IODINE AND OTHER ELEMENTS.
Iodine and Selenium
" Sulfur
44 Tellurium
44 Tin
(Pellini and Pedrina, 1908.)
(Olivari, 1908; Smith and Carson, 1908.)
(Jaeger and Menke, 1912.)
(van Klooster, 1912-13; Remders and de Lange, 1912-13.)
SOLUBILITY OF IODINE IN ARSENIC TRICHLORIDE. (Sloan and Mallet, 1882.)
t°. o°. 15°. 96°.
Gms. I per ico.gms. AsCl3 8.42 u.88 36.89
335 IODOEOSINE
IODOEOSIN (Sodium tetra iodofluorescein)
loo gms. H2O dissolve 90 gms. iodoeosin at 20-25°. (Dehn, 1917.)
100 gms. pyridine dissolve 4.63 gms. iodoeosin at 20-25°.
IOO gms. aq. 50% pyridine dissolve 71.6 gms. iodoeosin at 20-25°.
IODOFORM CHI3, IODOL C4I4NH (Tetraiodopyrrol).
SOLUBILITY IN SEVERAL SOLVENTS.
(U. S. P. VIII; Vulpius, 1893.)
Gms. per 100 Gms. Solvent.
Solvent. t°. , * —
Water 25 0.0106 0.0204
Alcohol 25 2.14(1.43 gms. (V.)) u.i
Alcohol b. pt. (10 gms. (V.))
Ether 25 19.2 (16.6 gms. (V.)) 66.6
Chloroform 25 ... 0.95
Pyridine 20-25 I73-1 ODehn, 1917.)
Aq. 50% pyridine 20-25 22-4
Lanolin (30% H20) 46 5.2 (Kiose, 1907.)
IRIDIUM CHLORIDE IrCU.
When i gm. iridium as chloride is dissolved in 100 cc. of 10% HC1 and shaken
at 1 8° with 100 cc. of ether, 0.02 per cent of the metal enters the ethereal layer.
When 20% HC1 is used 5% of the metal enters the ether. When dissolved in i %
HC1 or in water approximately o.oi per cent of the metal enters the ethereal layer.
(Mylius, 1911.)
IRIDIUM Ammonium CHLORIDE IrCl4.2NH4Cl.
SOLUBILITY IN WATER.
(Rimbach and Korten, 1907.)
Gms. IrCU-aNEUCl per 100 Gms. Gms. IrCU.aNH^Cl per 100 Gms.
I .
Water. Sat. Sol.
Water. Sat
.Sol.
'
14.4
o . 699 o . 694
52.2
I .
608 I.
583
26.8
o . 905 o . 899
61.2
2 .
I3O 2.
068
39-4
1.226 I.I24
69-3
2.
824 2.
746
IRIDIUM
DOUBLE SALTS
v
SOLUBILITY IN WATER.
(Palmaer — Ber. 23, 3817; 24, 2090, '91.)
Double Salt.
Formula.
t°.
Gnu
per
Irido
Pentamine Bromide
Ir(NH3)5Br3
12.5
O.
W
<i
U
Bromonitrate
Ir(NH3)sBr(N03)3
18
5.
58
«
It
Tri Chloride
Ir(NH3)5Cl3
i5-i
6.
53
U
11
Chloro Bromide
Ir(NH3)5QBr2
15
0.
47
n
«
Chloro Iodide
Ir(NH3)5ClI2
15
0.
95
K
U
Chloro Nitrate
Ir(NH3)5Cl(N03)2
15-4
i.
94
it
tt
Chloro Sulphate
Ir(NH3)5ClSO4.2H2O
15.0
0.
74
ft
tt
Nitrate
Ir(NH3)5(N03)3
16
0.
28
«
Aquo Pentamine Bromide
Ir(NH3)6(OH2)Br3
ord. temp.
25.0
«
«
Chloride
Ir(NH3)5(OH2)Cl3
ord. temp.
74.
7
«
tt
Nitrate
Ir(NH3)5(OH2)(N03)3
i?
IO.
o
IRON BROMIDE (Ferrous) FeBr2.6H2O.
SOLUBILITY IN WATER.
(Etard — Ana. chim. phys. [7] 2, 537, '94.)
A o Gms. FeBr2 A o
* ' per loo Gms. Sol.
Gms. FeBr2 t 0 Gms. FeBrs
per loo Gms. Sol. per 100 Gms. Sol.
— 20
47-0
30
55-o
60
59-o
0
50-5
40
56.2
80
61.5
20
5,3-5
IOO
64.0
IRON CARBONATE 336
IRON CARBONATE (Ferrous) FeCO3.
SOLUBILITY OF FERROUS CARBONATE IN AQUEOUS SALT SOLUTIONS, BOTH
WITH AND WITHOUT THE PRESENCE OF CARBON DlOXIDE.
(Ehlert and Hempel, 1912.)
(Each mixture was 1000 cc. in volume and was rotated constantly for 24 hours.
Temp., probably 5-8°.)
SOLUBILITY IN PRESENCE
OF CO2 (2 atmospheres pressure).
SOLUBILITY IN ABSENCE
OF CO2.
Aqueous Solution of:
r~
Cms. Salt per
1000 Cms. H2O.
Cms. FeCO3 per
1000 cc. Solvent.
Cms. Salt per Cms. FeC03 per
1000 Cms. H2O. 1000 cc. Solvent..
Water alone
0
6.I9I
NaCl
. . .
351-2
0-350
MgCl2.6H2O
86.9
5.840
«
700
4-555
tt
1150
4-459
. . .
. . .
tt
1437-5
4-693
. . .
. . .
n *
1725
5.398
. . .
. . .
tt
2300
9.052
2300
4-205
Na2S04.ioH20
137-7
7-943
137-7
0.701
a
Sat. at 14°
9-578
Sat. at 14°
0-934
MgSO4.7H2O
ioS-3
6.242
io5-3
1.467
tt
Sat. at 14°
7-392
Sat. at 14°
2-933
IRON BICARBONATE (Ferrous) Fe(HCO3)2.
SOLUBILITY OF FERROUS BICARBONATE IN CARBONATED WATER AT 30°.
(Smith, H. J., 1918.)
Pure white ferrous carbonate was prepared by heating to 100° for several
days in a steel bottle, an aqueous solution of ferrous sulfate, sodium bicarbonate
and carbon dioxide (introduced at 400 Ibs. pressure). The crystalline product
was similar to the mineral siderite and was probably isomorphous with calcite.
Fifty to one hundred gram portions were placed in a two- liter steel bottle, coated
on the inside with a mixture of beeswax and Venice turpentine. Water was added
and CO* introduced through a needle valve from a cylinder of the liquefied gas.
The pressure was read on a gauge. The bottle was rotated at constant tempera-
ture for several days or until equilibrium was reached. The portion of the
saturated solution for analysis was withdrawn through a brass tube attached to
the valve on the inside of the bottle and packed with cotton to act as a filter. The
filtered portion was received in a tared evacuated flask, containing a few cc. of
cone. HjSCX The CO2 was determined by absorption and the iron by precipitation,
resolution, reduction and titration with permanganate. The results show that
the decomposition tension of Fe(HCO3)2 is greater than 25 atmospheres at 25°.
Cms. Mols. per Liter.
Cms. per Liter.
Cms. Mols. per Liter.
Cms. per Liter.
•H2C03.
Fe(HC03)2.
'H2C03.
Fe(HCO3)2.
H2C03.
Fe(HC03)2.
H2C03.
Fe(HCO3)2.
0.1868
0
.00245
II
-58
0.436
0.3294
0
.00311
20
•43
0-553
0.1985
0
.00256
12
•3i
0-455
0-3745
0
•00315
23
•23
0.560
0.2168
0
.00262
13
•45
0.466
o . 4046
o
.00332
25
.09
0.590
0.2327
0
.00274
14
•43
0.487
0.4750
o
.00348
29
•45
O.6l9
o . 2960
0
.00303
18
•35
0-539
o . 6600
0
.00402
40
•93
0.715
0.3116
o
.00304
19
•32
0.541
0.7154
0
.00418
44
•36
0.744
0.3153
0
.00318
19
•55
0.566
0.7600
o
•00434
47
•13
0.772
IRON CHLORIDE (Ferrous) FeCl2.4H2O.
100 gms. sat. sol. in water contain 17.54 gms. Fe = 39.82 gms. FeCl2 at 22.8°.
loo gms. sat. sol. in water contain 18.59 gms. Fe = 42.8 gms. FeCl2 at 43.2°.
(Boecke, 1911.)
337
IRON CHLORIDE
IRON CHLORIDE (Ferrous) FeCl2.4H2O. SOLUBILITY IN WATER.
(Etard.)
10
IS
25
30
40
50
Gms. FeCl2
per 100 Gms.
Solution.
39-2
4O.O
41-5
42.2
43-6
45-2
Solid Phase.
t°.
60
80
87
90
100
120
Gms. FeCl2
per 100 Gms.
Solution.
47-o
50.0
51.2
51-4
51.8
Solid Phase.
FeCl2.4H2O+FeCl8
SOLUBILITY OF IRON CHLORIDE
(Roozeboom — Z. physik.
Mols.F<
t°. per 100 Mols,
H20.
Cms. FeCla per 100
Cms.
(FERRIC) Fe2Cl6 IN WATER.
Chem= 10, 477, '92.)
Gms. FeCla per too
Mols.
per 100
ols.
_, --
Gms.
H7O. Solution.
Solid Phase, Fe2Cl6.i2H2O.
-55 2.75 49-52 33-J2
-27 2.98 53.60 34-93
o 4-13 74-39 42-66
+ 20 5.10 91.85 47.88
30 5.93 106.8 51.64
37 8.33 150-0 60. 01
30 i i. 20 201.7 66.85
20 12.83 231.1 69.79
8 13.7 246.7 71.15
Solid Phase, Fe2Cl6.7H20.
20 11-35 204.4 67.14
32 13.55 244.0 70.92
30 15.12 272.4 73.13
25 15.54 280.0 73.69
Solid Phase, Fe2Cl6.sH2O.
12 12.87 231.8 69.87
27 14.85 267.5 72.78
35
50
55
55
j. H2O. Solution.
Solid Phase, FesCla-sHsO (con.).
15.64 281.6 73.79
17.50 315.2 75.91
19.15 344.8 77.52
20.32 365.9 78.54
Solid Phase, Fe2Cl6.4H2O.
50 19.96 359.3 78.23
55 20.32 365.9
60 20.70 372.8
69 21.53 387.7
73-5 25-0 450-2
70 27.9 502.4
66 29.2 525.9
Solid Phase, Fe2Cl&.
66 29.2 525.9
75 28.92 511.4
80 29.20 525.9
100 29.75 535-8
78.54
78.86
79-50
81.81
83.41
84.03
84.03
83.66
84.03
84.26
SOLUBILITY OF FERRIC CHLORIDE IN AQUEOUS SOLUTIONS OF
AMMONIUM CHLORIDE AT 25°, 35°, AND 45°.
(Mohr — Z. physik. Chem. 27, 197, '98.)
Results at 25°. Results at 35°. Results at 45°.
Mols. per
100 Mols. H2O.
Mols. per
100 Mols. H2O.
Mols. per
100 Mols. H2O.
NH4C1.
FeCl3.
NH4C1.
Fed,.
NH4C1.
FeCla.
O
10.98
O
J3-36
0-0
33-4
!-57
10-74
I.4I
13-05
2.48
9-02
3-08
9.28
4.08
9-58
5-28
7-73
6.98
7-64
. . .
9-59
6-77
10.76
6.70
13.09
6^31
9-83
6.70
II. 60
6-52
13-54
6.28
9-65
6.07
12.28
6.08
12.91
5-49
9-93
5-23
n-57
3-98
13-49
4.84
9-92
3-97
11.89
3-38
13.46
4.99
10.31
2.05
13-23
1-38
I3-30
0-0
14-79
o-o
i6!28
0-0
Solid Phase
in Each Case.
Fe2Cl«.i2H20(5.H2Oat4S0)
Hydrate + Double Salt
Double Salt
Double Salt + Mixed Ciystals
Mixed Crystals
IRON CHLORIDE
338
SOLUBILITY OF
FERRIC CHLORIDE IN AQUEOUS SOLUTIONS
OP
AMMONIUM CHLORIDE AT 15°.
(Roozeboom — Z. physik. Ch.
10, 148, '92.)
Mols. per 100 Mols.H2O.
Grams per ipo Gms.HjO.
Solid
NH4C1.
FeCl3.
'NHjCl. FeCl3>
Phase.
o.o
9-30
o.o 83.88
Fe2Cl«.i2H2O
1.09
9-57
3.24 86.32
44
1.36
9-93
4.03 9I.6l
Fe2Cl6.i2H20 -f Double Salt
2-OO
9.27
5.92 83.64
Double Salt
2-79
8.71
8.3I 78.77
"
4-05
8.09
12. 08 73. 2O
"
6.41
7.18
19.12 64.83
«4
10.78
6.21
32.04 56.00
"
7.82
6-75
23.21 60.83
Mixed Crystals containing 7.29%
FeCJ,
7.62
5-94
22.63 53.47
5.55
"
7.70
5-03
22.90 45-42
4-4
M
7.8l
4-34
23.23 39-I3
" M 3-8
It
S-52
2.82
25-33 25.43
1.64
<(
10.95
0.68
32.55 6-15
" " 0.31
II
u.88
o.o
35-30 o.o
NILC1
SOLUBILITY OF FERRIC CHLORIDE IN AQUEOUS HYDROCHLORIC ACID
SOLUTIONS AT DIFFERENT TEMPERATURES.
(Roozeboom and Schreinemaker — Z. physik. Chem. 15, 633, '94.)
Mols. per TOO
H,0.
Mols.
Gms. per 100 Gms. Mols
H20. Solid
. per 100 Mols
H20.
. Gms. per 100 Gms.
H20. Solid
HC1.
FeCl3.
HC1.
FeCl8. *****' HC1. FeCl3:
'HC1.
FeCl3. Phase
Results at o°.
Results at 25° (con.).
O
8
•25
0
74
3°
0.
0
29.00
0.0
26l.I
7-52
6
•51
15.22
58
62
7.
5
29.75
15.18
267.9
Fe2Cl6
13.37
6
-33
27.06
57
01
19.
35.25
39-46
317.4
•5 2M
16.80
8
-70
33-99
78
34
19.
5
35-25
39-46
3I7-4
18.45
10
•23
37-34
92
10
FeaCl« 20,
6
35-34
41.68
20.40
15
.40
41.28
138
7
.i2H203I>
34
41.58
63.42
374-4
^|u)
20.10
16
.00
40.67
144
i
33-
00
43-0°
66.77
387.3
19.95
17
•70
40.37
159
4
34-
65
44-80
70.11
403.4
19.00
22
•75
38.45
204
8
40.
4i
40.25
81.77
362.4
1 FeCl«
18.05
23
.41
36-53
210.
8 .
39-
03
41.38
78.98
372.7
[ C2.2HC1
18.05
23
.40
36-53
2IO.
8
^fflzO 35<
74
45-24
72-33
407.4
J + 4H2O
19.50
25
•93
39-55
233-5 J
Results at AO°.
24. 12
26.0O
26.00
34.60
37-27
34.60
30
32
32
36
38
.04
.16
.16
.11
.60
.11
48.81
52.60
52.60
70.01
75-41
70.01
270.
289.
289.
343-
329.
343-
i
6
2
6
2
F^fc>^4
Fe2HCl 2o °
-fW) 2°
32.4
37.45
37-45
50.80
58.0
50.8
0.0
27.11
27.11
54.64
o.o
54.64
291.7
337-3
337-3
457-5
522.3
457-5
1 Ferf*
Results at 25°.
42.
01
48.64
85.00
438. oj
O.O
IO
.90
o.o
98
IS^\ 42.
50
47-52
86.72
428.0
) Fe2Cl«
2-33
23
.72
4.715
213
6 r j 2 jf o 42 •
OI
48.64
85.00
438-0
i +4H2O
0.0
24
•5
0.0
220
7 J ''
0.0
2.33
7.50
23
23
29
•5
.72
-75
o.o
4.715
15.18
211.
267!
6 i Results for other temperatures
4 1 Fe2ci« are also given in the original
g f .yHaO paper.
0.0
31
•50
0.0
283.
6 J
339
IKON CHLORIDE
RESULTS FOR THE SYSTEM FERRIC OXIDE, HYDROCHLORIC ACID, WATER AT 25°.
(Cameron and Robinson, 1907.)
(Excess of ferric hydroxide was added to aq. ferric chloride solutions and agi-
tated for 3 months.)
Gms. per 100 Gms.
Sat. Sol.
Solid Phase. o f? £,
Gms. per too Gms.
Sat. Sol.
Solid Phase.
Fe2O3. HCl. FejOs.
HCL '
34
.61
59
.88
FeCl3.HC1.2HtO 1.485
21
.84
29
-33 {
FeCl3.6H20+
Fe203.*HCl.H2O
33
•27
60
•23
"
•349
16
.82
22
•55
Fe2Oa.itHCl.H2O
32
•78
54
+ FeCl3
.321
15
•83
21
.10
"
•95
58
.20
FeCV+FeCU^HjO
.284
14
.62
19
•53
«
34
.42
54
.12
FeCl3.2HjO
.242
12
•59
16.61
35
.22
59
.28
"
.220
II
.76
15
.28
•
34
.07
55
.71
I.I95
10
•56
13
.76
•
34
.21
55
•47
+FeCl3.2jH20 1.158
8
.60
II
.24
"
34
•44
51
.11
FeCl3.3JH20+ " I.H5
6
•47
8
•39
•
33
.04
46
.72
" +FeCl3.6H2O 1.070
4
.04
5
•36
(C
24
.42
33
.40
FeCU.6H20 1 . 047
2
•85
3
.66
"
Data for the systems FeCl2 + MgCl2 + KC1 + H2O at 22.8° and for FeCl2 +
KC1 + NaCl are given by Boeke, 1911.
100 gms. abs. acetone dissolve 62.9 gms. FeCl3 at 18°. (Naumann, 1904.)
100 gms. anhydrous lanolin (m. pt. about 46°) dissolve 4.17 gms. FeCl3 at 45°.
(Klose, 1907.)
DISTRIBUTION OF FERRIC CHLORIDE BETWEEN WATER AND ETHER AT 18°.
(Mylius, 1911.)
One-gram portions of iron as chloride were dissolved in 100 cc. of aq. HCl of
different concentrations and shaken with 100 cc. of ether in each case. The per-
centage of iron in the ethereal layer was determined after separation of the two
layers.
Per cent cone, of Aq. HCl i 5 10 15 20
Per cent of Iron Extracted by Ether (o.oi) o.i 8 92 99
Fusion-point curves (solubility, see footnote, p. i) for mixtures of FeCl3 + PbCl2
and FeCl3 + ZnCl2 are given by Herrmann, 1911, and for mixtures of FeCl3+TlCl
by Scarpa, 1912.
SOLUBILITY OF THE SALT PAIR FeCl3.NaCl IN WATER AT 21°.
(Hinrichsen and Sachsel, 1904-05.)
Gms. Used.
Gms. per 100 Gms.
Solution.
G. Mols.
per 100 Mols. H2O.
Solid Phase.
FeCl3.
NaCl.'
FeCl3.
NaCl.
FeCl3.
NaCl. "
0
3-6
0
36.10
0
II. 2
NaCl
1.8
3
24.27
9.10
2.69
2.8
Mix Crystals
3-6
2-5
25.40
8-45
2.81
2.6
tt
5-5
2
26.40
5-25
2.93
2-54
«
7.2
i-5
38.15
3.90-
4-23
1.22
tt
9
i
45.38
2-45
5-03
o-75
u
10.8
o-5
46.75
2. II
5-i8
0.65
tt
10.8
0
83.39
0
9-3
o
FeCla
IRON CHLORIDE
340
SOLUBILITY OF THE SALT PAIR FeCl3.KCl IN WATER AT 21°.
(Hinrichsen and Sachsel, 1904-05.)
Cms. Used.
Fed,.
O
13
18
23
28
KCl.
35
28
21
16
36.2 9
46.5 6
155 o
Gms. per 100 Gms.
Solution.
Gms. Mols. per 100
Mols. H20.
Solid Phase.
FeClj.
O
13-44
23.18
28.05
KCl. '
34-97
24-45
16.54
11.69
FeCl3.
0
1.49
2-57
3-«
KCl.
8-45
5-90
3-99
2.82
KCl
Mix Crystals
35-72
11.68
3-96
2.82
"
36.62
11.19
4.06
2.70
FeCl3.2KCl.H20
37-35
13.67
4.14
3-30
a
51.69
7-54
5-73
1.82
a
83-89
0
9-3
0
. FeCl3
SOLUBILITY OF THE SALT PAIR FeCl3.CsCl IN WATER AT 21°.
(H. and S.)
Gms. Used.
Gms. per 100 Gms.
Solution.
Gms. Mols. per 100
Mols. H,0.
Solid Phase.
FeCl3.
CsCl.
' FeCl3.
CsCl.
FeCl3.
CsCl. '
O
65
0
65
0
6-95
CsCl
0.6
ii. 6
0-45
55-18
0.05
5-9
FeCl3.3CsCl.H2O
1-4
10.2
2.1
52.38
0.23
5-6
ts
2.2
8.8
5-24
5J-44
o-57
5-5
((
2
74
7-8
47.70
0.86
5-i
FeCl3.2CsCLH2O
3-8
6
8-93
4i-i5
0.99
4-4
u
4-6
4-6
15-34
25-25
1.70
2.7
n
5-4
2.8
21.65
14.96
2.40
1.6
(i
6.2
1.4
27.96
8.42
3.10
0.9
ti
35
0.2
48.71
0.94
5-40
O.I
n
35
0
83-89
o
9-3
o
FeCla
IRON FORMATE (Ferric) Fe3(OH)2(HCOO)7.4H2O.
SOLUBILITY IN WATER AND IN ABSOLUTE ALCOHOL.
(Hampshire and Pratt, 1913.)
15
20
25
30
35
Solubility in Water.
Gms. Salt
per 100 Gms. Solid Phase.
H20.
Fe3(OH)2(HCOO)74H2O
Solubility in Abs. Alcohol.
Gms. Salt
t°. per 100 Gms.
QH6OH.
5-08
5-52
6.10
6.78
7-52
19
22
23
4-59
6.25
7.62
(The sat. solutions are not stable.)
341
IRON HYDROXIDE
IRON HYDROXIDE (Ferric) Fe(OH)3.
SOLUBILITY OF FERRIC HYDROXIDE IN AQ. OXALIC ACID SOLUTION AT 25°.
(Cameron and Robinson, 1909.)
The solutions were constantly agitated for 3 months. The solubility is directly
proportional to the concentration of the oxalic acid and no definite basic ferric
oxalate is formed.
Gms. per 100 Gms. Sat. Sol.
Fe2O3. CA
0.48 0.61
0.95 1.23
1.86 2.45
Gms. per 100 Cms. Sat. Sol.
Sat. Sol.
1.007
I.OI5
I.03I
Sat. Sol.
1.040
1.050
1.064
2-33
2.98
3.62
5.17
IRON NITRATE (Ferric) Fe(N03)3.9H20.
EQUILIBRIUM IN THE SYSTEM, FERRIC OXIDE, NITRIC ACID AND WATER AT 25°.
(Cameron and Robinson, 1909.)
Solutions of ferric nitrate of varying concentrations were shaken with freshly
precipitated ferric hydroxide at const, temp., 25°, for 4 months. The acid branch
of the curve was studied in a similar manner by starting with ferric nitrate and
various concentrations of nitric acid. No definite basic nitrates of iron were
formed.
^25 Of |
Gms
. per 100 Gms.
Sat. Sol. solid Phase. • c.
dys of
it Sol
Gms. per 100 Gms.
Sat. Sol. •
Solid Phase.
Fe2O3. N2O5.
,t. OUl.
' FeA.
NA.:
.032
I
.78
2
.21 FeA m NA n H2O
I
•452
12
.14
33-
5
FeA.3NA.i8HjO
:°79
3
•99
5
.61
I
•434
9
•95
36.
3
"
.127
5
•79
9
"
I
.417
7
•25
40.
3
"
.177
7
.22
12
.31
I
.404
5
.02
47-
5
"
.264
9
.70
16
.60
I
.428
3
•55
51.
5
"
.368
12
.48
22
.70
I
•450
4
.51
52
*
•435
14
.62
28
•13
I
•465
4
•19
55-
2
"
.498
15
.40
29
.52
I
.407
3
•93
47-
2
FeA.4NAi8H20*
.496
15
.22
30
.50 FeA.3N205.i8H20
I
.419
3
•52
49-
6
"
This salt was obtained accidentally and its preparation could not be repeated.
IRON NITRATE (Ferrous) Fe(NO3)2.6H2O.
SOLUBILITY IN WATER.
(Funk, 1900.)
t°.
27
21.5
19
15.5
Gms.
Fe(NOs)2
per 100
Gms.
Sol.
35-66
36.10
36.56
37-17
Mols.
Fe(NO3)2
per 100
Mols.
H20.
5-54
5-64
5-76
5-9i
Solid Phase.
Gms.
Mols.
Fe(N03)2
Fe(NO^
t°.
per 100
Gms.
per 100
Mob
Sol.
H20
-9
39-68
6.$7
0
4L53
7.10
18
45-14
8.23
24
46.51
8.70
Solid Phase.
Fe(NOl)2.6HlO
60.5 62.50 16.67
Density of solution saturated at 18° = 1.497.
IRON OXALATE 342
IRON OXALATE (Ferrous) FeC204.2H2O.
SOLUBILITY IN WATER>T 25° DETERMINED BY THE CONDUCTIVITY METHOD.
(Schafer, 1905.)
The sat. solution contains 5.38. 10-* gm. mols. C2O4 per liter.
IRON OLEATE.
100 gms. glycerol (d = 1.114) dissolve 0.71 gm. iron oleate. (Asselin, 1873.)
IRON OXIDES, HYDROXIDE and SULPHIDE.
SOLUBILITY IN AQUEOUS SUGAR SOLUTIONS.
(Stclle — Z. Ver Zuckerind. 50, 340, 'oo.)
% <?IIMT One Liter of Sugar Solutions Dissolves Milligrams of:
te Sol- Feg(OH)6 at; Fe?O3 at: _ Fe3O4 at: _ FeSatt
vent. i7.4<>. ^ 5?. 17.5°.' 4!* ' 17.5°- 45^ 75°^ 17-5°. ^ 7?T
10 3.4 3-4 6.1 1.4 2.0 10.3 10.3 12.4 3.8 3.8 5.3
30 2.3 2.7 3.8 1.4 ... 12.4 10.3 12.4 7.1 9.1 7.2
50 2.3 1.9 3.4 0.8 i.i 14.5 10.3 14-5 9-9 19-8 9.1
IRON PHOSPHATE Fe2(PO4)3.
THE ACTION OF WATER AND OP AQUEOUS SALT SOLUTIONS UPON
FERRIC PHOSPHATE.
(Lachowicz — Monatsh. Chem. 13, 357, '92; Cameron and Hurst — J. Am. Chem. Soc. 26, 888, '04.)
The experiments show that the ordinary precipitation methods for
the production of ferric phosphate give products which do not conform
to the formula Fe2(PO4)3. By digesting such samples with water
very little is dissolved, but the material is decomposed to an extent
depending upon the relative amounts of solid and solvent used. The
amount of PO4 dissolved per gram of Fe2(PO4)3 varies from about
0.0026 gram removed by 5 cc. H2O to 0.0182 gram removed by 800 cc,
H2O at the ordinary temperature.
SOLUBILITY FERRIC PYROPHOSPHATE IN AQ. AMMONIA AT o°. (Pascal, 1909.)
The solutions containing an excess of salt were agitated violently every half
hour for seven hours and filtered at o°. The sat. sol. was analyzed for ammonia
and for residue obtained by evaporation.
Gms.NH3 F<.{??n Gms.NH3
P^Sol"13' Pe^ioo^s. Solid Phase. P^gms. pem's. Solid Phase.
0.884 5.606 Fe«(PA)i •••5*92 14-71 viscous black deposit
1.59 9-75 " 8.26 13.89 chamois colored lumps
3.71 14-85 " 10.55 7.40
4.72 15.94 15.96 2.52
5.93 I3-92 viscous black deposit 18.83 °-445
7.91 14.61
SOLUBILITY OF FERRIC PHOSPHATE IN AQ. PHOSPHORIC ACID SOLUTIONS AT 25°-
(Cameron and Bell, 1907.)
Solid ferric phosphate of unknown composition was constantly agitated with
aq. phosphoric acid solutions of concentrations up to 5% for 4 months. Analy
of the sat. solutions and solid phases were made.
ses
^of
Gms. per 100 Gms. Sat. Sol.
Solid Phase.
Sat.' Sol.
.0074
.0162
.0244
.0310
•0383
FeA- PA. '
O.OIO5 0.942
0.0205 1-984
0.0384 2.838
0.0611 3.770
0.0849 4.706
Solid Solution
it
343
IRON SULFATB
SOLUBILITY OF FERROUS SULFATE
IN WATER.
(Fraenckel, 1907.)
Gms. FeSO4
Gms.
f
per 100 Solid Phase.
Gms.H2O.
t°. FeSO4penoo Solid Phase.
Gms. H2O.
— o.
172
I.OI56 Ice
45
.18
44
•32
FeSO4.7H2O
— o.
566
4.2^2
50
.21
48
.60
"
— I .
063
8.7054
52
50
.20
"
— I .
511
12.713
54-03
S2
.07
"
— I.
771
14.511
56
.56 ti
r. pt«54 .
58
(1 I T7|»Cf\ .
H,0
— I .
82Eutec
.17.53 Ice+FeS04.7H20
60
.OI /
54
•95
FeS04.4H2O
0
15.65 FeS04.7H20
65
55
•59
" unstable
+ 10
20.51
70
.04
56
.08
" "
15-
25
23.86
64
.8tr.
Pt.
. . FeSO4.4H2O+FeSO4.H2O
20.
13
26.56
68
.02
52
•31
FeSO4.H2O
25-
O2
29.60
77
1
45
.90
"
30.
03
32.93
80
.41
43
-58
"
35-07
36.87
85
.02
40
.46
"
40.
05
40 . 2O "
90
-13
37
.27
"
<Zl6.6
of sat.
sol. = 1.219]
(Greenish and Smith,
1903.)
SOLUBILITY OF FERROUS SULFATE IN AQ. SOLUTIONS OF LITHIUM SULFATE AT 30°.
AND VICE VERSA. (Schreinemakers, 1910.)
Cms. per 100 Cms. Sat. Sol."
' FeS04.
24.87
Li2SO4.
0
FeSO4.7H2O
24-45
4
tt
21.15
5-58
(i
18.79
ii. 16
a
16.51
15.81
u
16.11
16.50
11 +Li2S04.
Gms. per 100 Cms. Sat. Sol.
FeSO4.
15-39
12.68
5-32
3-74
o
Li2S04.
16.80
18.31
22.15
23-I5
25.1
Solid Phase.
Li2SO4.H2O
EQUILIBRIUM IN THE SYSTEM FERRiCiOxiDE, SULFURIC ACID AND WATER AT 25°.
(Cameron and Robinson, 1907.)
(Excess of freshly precipitated ferric hydroxide was added to ferric sulfate solu-
tions of varying concentrations and the mixtures constantly shaken for 4 months.)
d
c~
25 Of
t Snl
Gms. per 100 Gms.
Sat. Sol.
Solid
Phasp
Gms. per
Sat.
100 Gms.
Sol.
Solid
Phase.
OU
L. OOl.
Fe203.
S03/
jrnase.
Fe2O3. SO3.
I
.001
0
.07
o
.11
Solid Solution
20
.48
26.
18
Fe2O3.3SOs. ioH20
I
.Oil
O
.62
0
-94
"
*9
•77
28.
93
it
I
•045
2
•03
2
-65
u
10
.87
31.
35
Fe2O3.4S03ioH2O
I
.131
6
.18
7
.40
t(
0
.16
tt
I
.217
IO
•03
ii
.84
0.07
41.
19
u
I
.440
15
.90
20
.70
M
I
•05
42.
43
t(
SOLUBILITY OF FERRIC SULFATE AND OF FERROUS SULFATE IN AQ.
SOLUTIONS OF SULFURIC ACID AT 25°. (Wirth, 1912-13.)
Results for Ferric Sulfate. Results for Ferrous Sulfate.
Normality of
used Acid.
2.25
6.685
19.84
Gms. per 100 Gms. Sat.
Sol.
Normality o
used Acid.
2.25
10.2
12.46
I5-I5
19.84
, Gms. per 100 Gms. Sat.
f Sol.
Solid Phase.
FeSO4.7H2O
a
FeS04.H2O
tt
«
FeA
9-99
5-82
O.O2
= Fe2(S04)3.
25.02
14.58
0.05
FeA =
IO
5-414
3.8l6
2. II
0.08
FeS04.
19.03
10.30
7.26
4.015
0.1522
IRON SULFATE
344
EQUILIBRIUM IN THE SYSTEM FERRIC OXIDE-SULFUR TRIOXIDE- WATER AT 25°.
(Wirth and Bakke, 1914.)
(The mixtures were shaken for 3-4 weeks.)
Gms. pe
Si
;r 100 Gms.
t. Sol.
Solid Phase,
not det.
prob. Fe2(S04)3.H2S04.9H20
+Fe2(S04)3.H2S04.3H20
Fe2(SO4)3.H2SO4.8H2O
" +Fe(S04)3.H2S04.3H20
Fe(S04)3.H2SO4.8H2O
unstable
Gms
.per
Sat.
100 Gms.
Sol.
Ft
O
3
6
9
12
13
13
.24
•53
•65
•39
•03
•27
.68
S03.
7I-23
56.84
» 1
32.15
31-54
3I-84
31-78
Fe2(
14.
20.
9-
II.
13-
16'
49
21
39
06
88
07
S03.
31-45
31.88
3I-30
31-54
29-43
28.33
27.92
27.98
Solid Phase,
unstable
Fe2(SO4)3.H2S04.8H2O+
Fe2(S04)3.9H20
Results are also given for the two forms of yellow ferric sulfate (a copiapite and
0 copiapite) also for ferric hydroxide and sulfate solutions.
It was found that a saturated solution of Fe2(SO4)3.H2SO4.8H2O in abs. alcohol
at 25° contained 8 gms. Fe2O3 + 17.18 gms. SO3 (Ratio, 1 14.235) per 100 gms. sat.
sol.
The yellow ferric sulfate Fe2(SO4)3.9H2O is less soluble in alcohol. After 4
weeks shaking at 25°, 100 gms. of the sat. solution in abs. alcohol contained 4.497
gms. Fe2Os and 6.779 Sms- SOs (Ratio, 1:3.006). Thus the alcoholic solution,
just as the aqueous, is considerably more acid than the solid phase with which it
is in equilibrium.
loo grams sat. solution in glycol contain 6 gms. FeSO4 at ordinary temperature.
(de Coninck.)
100 gms. anhydrous hydrazine dissolve I gm. ferrous sulfate at room temp,
with decomposition. (Welsh and Brodeison, 1915.)
SOLUBILITY OF MIXTURES OF FERROUS SULPHATE FeSO4.7H2O AND
SODIUM SULPHATE Na2SO4.ioH2O IN WATER.
(Koppel — Z. physik. Chem. 52, 405, '05.)
Solid Phase.
FeS04.7H20 + Na2S04.ioH«0
FeNa2(S04)24H20
M
M
FeNaaCSOOz^HsO + FeSO4.7H20
t°.
Gms. per 100 Gms,
Solution.
Gms. per 100 Gms.
If20.
FeSO4.
Na2S04.
FeSO4.
Na2SO4.
0
14
•54
4
•93
18
.06
6
.11
15-5
17
.76
II
•32
25
•05
15
•97
21.8
16
•57
15
24
•34
22
•51
24.92
16
.21
1$
.13 23.62
22
.04
35
16
•35
14
.98
23
.91
21
•83
40
16
•37
15
.42
24
.01
22
.62
18.8
18
•13
I3.8
26
•63
2O
.28
23
19
•58
12
•5
28
.82
18
•4
27
20
•97
II
•3
30
•95
16
.64
31
22
.91
9
.71
33
•99
14
.41
35
23
•85
9
.26
35
.66
13
•85
40
26
•32
7
•85
39
.98
II
.92
18.8
18
•23
14
•83
27
•23
22
.16
23
13
•83
18
.04
20
•31
26
.48
28
7
.66
24
.41
ii
.28
35
•94
31
4
•58
29
•5°
6
•95
44
•75
35
4
.04
30
•49
6
.16
46
•58
40
4
.10
30
.60
6
.27
46
•99
FeNa2(SO4)24H2O + N
FeNa3S044H20 -f NajSO*
345 IRON SULFATE
IRON Potassium SULFATE (Ferrous) FeSO4.K2S04.6H2O.
SOLUBILITY IN WATER. (Tobier, 1855.)
f0 Gms. K2Fe(SC>4)2 t» Gms. K2Fe(SO4)2
per 100 Gms. H2O. per 100 Gms. H20.
o 19-6 35 41
10 24.5 40 45
14-5 29.1 55 56
16 30-9 65 57.3
25 36-5 70 64.2
IRON SULFIDE (Ferrous) FeS.
One liter of water, saturated at 18° with precipitated ferrous sulfide, contains
70.I.IO"6 mols. FeS = 0.00616 gm., determined by conductivity method.
(Weigel, 1906, 1907.)
Additional data for the solubility in water are given by Bruner and Zawadzki.
loo gms. anhydrous hydrazine dissolve 9 gms. FeS at room temp, with decom-
position. (Welsh and Broderson, 1915.)
Fusion diagrams for mixtures of FeS + PbS and for FeS + ZnS are given by
Friedrich, 1907, 1908.
IRON SULFONATES.
SOLUBILITY OF IRON PHENANTHRENE SULFONATES IN WATER AT 20°.
(Sandquist, 1912.) Gms Anhydrous Salt
Salt' per 100 Gms. H2O.
Iron 2-Phenanthrene Monosulfonate sH^O o . 044
" 3- " " 5H20 0.20
" lo- 6H2O 0.16
IRON THIOCYANATE (Ferric) Fe(CNS)3-3H2O.
DISTRIBUTION BETWEEN WATER AND ETHER. (Hantzsch and Vagt, 1901.)
Results at 25°. Results at Several Temperatures.
Gm. Mols. Fe(CNS)3 per Liter. c Gm. Mols. Fe(CNS)3 per Liter. ,.
H2O Layer (c). Ether Layer (cO- c> H2O Layer (c). Ether Layer (c1) . c'
0.0202 0.0108 1.87 o 0.0089 0.0167 °-532
0.0119 0.0034 3.51 10 0.0127 0.0128 0.995
0.0066 0.00093 7-°7 20 0.0165 0.0091 1.814
0.0035 0.00025 J3-95 3° 0.0196 0.0059 3.303
35 0.0207 0.0048 4.32
Results for the effect of HNO3 upon the distribution at 25° are also given.
ITACONIC ACID CH«:C(COOH)CH,COOH.
Data for the distribution of itaconic acid between water and ether at 25° are
given by Chandler, 1908.
KERATIN.
100 gms. H2O dissolve 8.71 gms. keratin at 20-25°. (Dehn, 1917.)
100 gms. aq. 50% pyridine dissolve 16 gms. keratin at 20-25°. "
Pyridine mixes with keratin in all proportions at 20-25°. "
' SOLUBILITY IN WATER, (von Antropoff, 1909-10.)
(Results in terms of coefficient of absorption as defined by Bunsen, see p. 227, and
modified by Kuenen in respect to substituting mass for volume of water involved.)
t°. Abs. Coef. (First Series). Abs. Coef. (Second Series).
o 0.1249 0.1166
10 0.0965 0.0877
20 0.0788 0.0670
30 0.0762 0.0597
4O O.O74O 0.0561
50 0.0823 0.0610
The cause of the differences between the first and second series of results was
not ascertained by the author.
LACTIC ACID
346
LACTIC ACID (t) CH3CHOHCOOH.
DISTRIBUTION BETWEEN WATER AND ETHER.
(Pinnow, 1915.)
Results at 27.5°.
Results at 15°.
Gm. Mols. Acid per Liter:
Gm. Mols. Acid per Liter:
(w)
HjO Layer (w).
Ether Layer (e).
e
H20 Layer (w).
Ether Layer (e).
(«)
I.98
0.215
9.19
1-354
0.130 -
10.42
I-3SI
0-133
10.15
0.3203
0.0278
11.52
0.297
0.0246
12. 08
0-1855
0.0156
11.89
0.1448
O.OIlS
12.27
0.0548
O.0046
11.88
F.-pt. data for mixtures of trichlorolactic acid and dimethylpyrone are given by
Kendall, 1914.
LACTOSE (see sugars, pages 695-7).
LANTHANUM BROMATE La(BrO3)s.9H2O.
100 gms. H2O dissolve 28.5 gms. lanthanum bromate at 15°. (Marignac.)
LANTHANUM CITRATE 2(LaC2H6O7).7H2O.
100 gms. aq. citric solution containing 10 gms. citric acid per 100 cc., dissolve
0.8 gm. La(C6H6O7) at 20°. (Holmberg, 1907.)
LANTHANUM CobaltiCYANIDE La2(CoC6N6)2.9H2O.
100 gms. aq. 10% HC1 (dm = 1.05) dissolve 10.41 gms. salt at 25°.
(James and Willand, 1916.)
LANTHANUM GLYCOLATE La(C2HsO3)3.
One liter H2O dissolves 3.328 gms. La(C2H3O3)3 at 20°. (Jantsch'and Grunkraut, 1912-13.)
LANTHANUM IODATE La(I03)3.
SOLUBILITY IN WATER AND IN AQ. SALT SOLUTIONS AT 25°.
(Harkins and Pearce, 1916.)
1000 gms. H2O dissolve 0.6842 gm. La(IO3)3 at 25°, dap sat. sol. = 0.99825.
•" ~
Cone, of
Gms.
^ of
Cone, of
Gms.
, f
Salt.
Salt, Milli-
Li(IO3)3
Salt. Salt, Milli-
*! -
Nonnal.
per Liter.
Sat. Sol.
Normal.
per Liter.
Sat. Sol.
La(NO,),
2
0-5595
0.99732
NaNO3 25
0.86901
.00250
"
5
0.5288
0.99807
So
0.99040
.00385
ti
10
0.5194
0.99859
IOO
I . 1603
.00742
"
50
0.5522
I. 00212
200
I-385
.01290
u
IOO
0.6214
I. OO66I
400
1.636
.02422
'n
200.52
0.7431
I.OI533
800
2. 156
.04677
KIO,
0.0990
0.6290
I.OOO3O
I6OO
2.859
.09005
14
0.4957
0.5633
1.00027
" 32OO
3.030
.17243
It
K
0.9914
1.9828
0.4970
0.3738
1.00030
I.0003I
^N^O 1 26^4
0.631
.00112
NalO,
0.0913
0.63538
I.0006o
52.68
0-674
.00355
"
0.4560
o . 56466
I.OOO59
105.36
0-754
.00971
1C
0.9130
0.50835
1.00065
158.04
0.816
.01608
u
I . 8260
0.39938
1.00065
196.83
0.867
.02183
U
3.6530
0.19736
1.00069
393.67
1.063
.04343
u
4.5326
0.13393
1.00083
787.35
1-364
.08286
(i
6.7989
0.09733
I.OOI3O
I574-70
1.923
.16652
According to Rimbach and Schubert (1909), one liter H2O dissolves 1.681 gms.
Li(IO3)3 at 25°, determined chemically, and 1.871 gms. determined electrolytically;
solid phase, 2La(IO,)3.3H2O.
LANTHANUM MALONATE La2(C3H2O4)3.5H2O.
100 gms. aq. Am. malonate sol. (10 gms. per 100 cc.) dissolve 0.2 gm. ) La2(C3H2O4)s
loo gms. aq. malonic acid sol. (20 gms. per loocc.) dissolve 0.6 gm. f at 20°.
(Holmberg, 1907.)
347
LANTHANUM MOLYBDATE
LANTHANUM MOLYBDATE La2(MoO4)3.
One liter H2O dissolves 0.0179 gm- La2(MoO4)3 at 25° and 0.0332 gm. at 85°.
(Hitchcock, 1895.
LANTHANUM Ammonium NITRATE La(NO3)3.2NH4NOs.
100 gms. H2O dissolve 181.4 gms. La(NO3)3.2NH4NO3 at 15°. (Holmberg, 1907.)
LANTHANUM j Double. NITRATES.
SOLUBILITY OF LANTHANUM DOUBLE NITRATES IN CONC. HNO3(dia = 1.325)
AT 1 6°. (Jantsch, 1912.)
Salt.
Lanthanum Magnesium Nitrate
Nickel
Cobalt
Zinc
" Manganese "
Formula.
[La(N03)6]2Mg3.24H20
Co3 "
Zn3 "
Mn3 "
Gms. Hydrated Salt
Dissolved per
Liter Sat. Sol.
63-8
80.3
109.2
124.1
LANTHANUM NITRATE La(NO3)3.
SOLUBILITY OF LANTHANUM NITRATE IN AQUEOUS SOLUTIONS OF LANTHANUM
OXALATE AT 25° AND VICE VERSA. (James and Whittemore, 1912.)
Gms. per ioo Gms. Sat. Sol.
Solid Phase.
Gms. per 100 Gms. Sat. Sol.
La2(C204),.3H20
O
0.67
2.IO
2.23
2.26
2-34
2-47
2-59
2.68
not det. not det.
La;(C204)3.
La(NO3)3. '
ooiia rnase.
not det.
not det.
La2(C204)3.5H20
3-32
42.27
La2(C204)3.8H20
2.80
38-50
"
2.51
35-57
"
2.21
31-53
ft
2.01
28.63
«*
I.46
22.15
«
1.18
17.99
H
0.50
9.89
«
0.28
5-o6
H
La(N03)3.
60.17 LatNOa),
59-91
59-03 "
59-03
58.22
55-20
52-74
49.84
45-26
La2(C204)3.SH20
LANTHANUM OXALATE La2(C2O4)3.9H2O.
One liter water dissolves 0.00062 gm. La2(C2O4)3 at 25°, determined by electroly-
tic method. (Rimbach and Schubert, 1909.)
ioo gms. aq. 10.2% HNO3 (d = 1.063) dissolve 0.80 gm. La2(C2O4)3 at 15°.
(v. Scheele, 1899.)
ioo gms. aq. 19.4% HNO3 (d = 1.116} dissolve 2.69 gms. La2(C2O4)3 at 15°.
(v. Scheele, 1899.)
SOLUBILITY OF LANTHANUM OXALATE IN AQ. SOLUTIONS OF SULFURIC
ACID AT 25°. (Hauser and Wirth, 1908; Wirth, 1908; Wirth, 1912.)
Normal- Gms. per ioo Gms. Normal- Gms- P61" Joo Gms.
ity of Sat. Sol. Solid Phase. ity of Sat. Sol. Solid Phase.
H*SO4. La2O3 = La2(C204)3. H2SO4. La2O3
o.i 0.0208 0.0346 La2(C2O4)3.9H2O 2
0.5 0.0979 0.1629
La2(C2O4)3.
0.4417 0.7344 La2(C2O4)3.9H20
3.09 0.680 1.1306
4.32 0.880 1.4630
5.6 1.092 1.8155 "
0.2383 0.3962
c.S 0.319 0.5304
SOLUBILITY OF LANTHANUM OXALATE IN AQ. SOLUTIONS OF OXALIC ACID
AT 25°. (Hauser and Wirth, 1908.)
Normality of Aq. Gms. per ioo Gms. Sat. Sol. Solid phase
La2(C204)3.
Oxalic Acid.
o . i unweighable
i.o 0.00032 0.00053
3.2 (sat.) 0.00045 0.00075
Results are also given for the solubility in mixtures of sulfuric and oxalic acids,
ioo cc. aq. 20% triethylamineoxalate dissolve approx. 0.032 gm. La2(C2O4)3.
(Grant and James, 1917.)
LANTHANUM PHOSPHATE
348
LANTHANUM Dimethyl PHOSPHATE La2[(CH,)jPO4]6.4HjO.
100 gms. H2O dissolve 103.7 gms. La2[(CH3)2PO4]6 at 25°. (Morgan and James,li9t4.)
LANTHANUM SULFATE La2(SO4)3.9H2O.
SOLUBILITY IN WATER. (Muthmann and Rolig, 1898.)
Gms. La2(SO4)3 per 100 Gms.
Solution. Water.
2.91 3
2.53 2.6
Gms. La2(SO4)3 per 100 Gms.
Solution/ Water.
o
14
30
1.86
1.9
5°
75
100
o-95
0.68.
0.96
0.69
SOLUBILITY OF LANTHANUM SULFATE IN AQ. SOLUTIONS OF AMMONIUM
SULFATE, POTASSIUM SULFATE AND SODIUM SULFATE. (Ban-e, 1910, 1911.)
In Aq. (NH4)2SO4 at 18°. In Aq. K2SO4 at 16.5°. In Aq. Na2SO4 at 18°.
Gms. per 100 Gms. H2O. Solid
Gms. per 100 Gms. H2O. Solid Gms. per 100 Gms. H2O.
Solid
(NH4)2SO4. La2(S04)3. phase-
K2SO4. La2(SO4)3. Muse. NazSCv La2(SO4)3.
Phase.
4.01
0.393 I.I-2
o 2.198 1.0.9 ° 2.130
1.0.9
8-73
0.279
0.247 0.727 1. 1.2 0.395 0.997
I.I. 2
18.24
0-253
0.496 0.269 0.689 0-353
11
27.89
0.476* "
0.846 0.185 0-774 0.299
(t
36.11
0.277* "
1.029 0.054 1.5 1.136 0.129
ti
47-49
0.137 2.5
1.156 0.022 " 2.480 0.044
"
53-82
0.067 1.5
3.802 0.019
it
65.29
0.0117
5.548 0.016
"
73-78
. 0.0033
* = unstable equilibrium.
1.0.9
KorN;
= La2(S04)3.9H20,
a), 2.5 = 2La2(S04)
1. 1.2 = La2(SO4)3.*2SO4.2H2O (where X =
3.5(NH4)2S04, 1.5 =JLa2(S04)3.5*2S04.
(NHO,
SOLUBILITY OF LANTHANUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 25°. (Wirth, 1912.)
Normality
of Aq.
H2S04.
Gms. per 100 Gms.
Sat. Sol.
pS. Ng-ty
Gms. per 100 Gms.
Sat. Sol. ^Solid
1^03 =
La2(S04)3.
La203 =
= La2(S04)3.
Water
I
•43
2
•483
La2(S04)3.9H20 4
.321
I
.11
I
.927 LajCSOJs.gl
o
•505
I
.69
2
•934
6
.685
0
•531
0
.9217
i
.10
I
.796
3
.118
9
.68
O
.266
O
.4617
2
.16
I
.818
3
•156
12
.60
0
.214
o
•371
3
•39
I
.42
2
-465
15
•15
0
.177
0
•307
Data for the solubility of lanthanum sulfate in aq. H2SO4 in presence of solid
oxalic acid at 25° are given by Wirth, 1908.
LANTHANUM SULFONATES.
SOLUBILITY OF EACH IN WATER.
Sulfonate.
Lanthanum Benzene Sulfonate
m Nitrobenzene Sulfonate
' m Chlorbenzene Sulfonate
m Brombenzene "
Gms.
Anhydrous
Formula. Sulfonate Authority.
per too
Gms. H2O.
63 . 1 (Holmberg, 1907.)
16
La[C«H6SO3]3.9H2O
La[C6H4NO2SO3]3.6H2O
LafCjH4Cl.SO3ls.9H2O
LalC6H4Br.SO3l3.9H2O
I3-I
12.9
' (6) Chloro (3) Nitrobenzene (i) )Sulfo-j La[C6H3Cl(NO2)SO3]3.8H2O 24 . 5 "
' (i) Bromo (4) Nitrobenzene (2) { nate \ LalCgHjBrNOzSO^.SHzO 5 (Katz & James, '13.)
*' a Naphthalene Sulfonate La[C10H7SO3]3.6H2O 5 . 2 (Holmberg, 1907.)
" 1.5 Nitronaphthalene Sulfonate La[CioH8(NO2)SO3l3.6H2O 0.55 "
"1.6 " " « .9H.D 0.21
" 1.7 " " " .9IW) i.i
349 LANTHANUM TARTRATE
LANTHANUM TARTRATE La2(C4H4Oe
One liter H2O dissolves 0.059 gm. La2(C4O4O6)3 at 25° (solid phase La2(C4H4O6)3.
3H2O). Determined by electrolytic method. (Rimbach and Schubert, 1909.)
SOLUBILITY OF LANTHANUM TARTRATE IN AQ. TARTARIC ACID AND AMMONIUM
TARTRATE SOLUTIONS AT 20°.
(Holmberg, 1907.)
In Aq. Tartaric Acid. In Aq. Ammonium Tartrate.
Gms. Tartaric Acid per Gms.La^C^O^sper • Gms. Am. Tartrate per Gms. La^C^O^s per
100 cc. Solvent. too Gms. Sat. Sol. 100 cc. Solvent. 100 Gms. Sat. Sol.
20 0.6 10 0.2
40 1.2 20 0.6
LANTHANUM TUNGSTATE La2(WO4)3.
One liter H2O dissolves 0.0117 gm. La2(WO4)3 at 27° and 0.0236 at 65°.
u (Hitchcock, 1895.)
LAURIC ACID Ci2H23COOH.
SOLUBILITY IN ALCOHOLS.
(Timofeiew, 1894.)
Alcohol t° Gms.CuH-aCOOHDer Alcohol t° Gms. C,2H23COOH per
Alcohol. t . IQO Gms Sa(. Sol Alcohol. t . IQQ Gms Sat sd
Methyl Alcohol o 14.8 Propyl Alcohol o 21.5
21 58.6 21 52.6
Ethyl Alcohol o 20.5 Isobutyl Alcohol o 18.4
21 57.3 21 49.7
LEAD Pb.
An extensive investigation of the solubility of lead in the water passing through
lead pipes is described by Paul, Ohlmiiller, Heise and Auerbach, 1906. ^ The
solubility is increased by oxygen, CO2, sulfates and perhaps other salts; it is de-
creased by hydrocarbonates.
SOLUBILITY OF LEAD IN LIQUID AMMONIA-SODIUM SOLUTIONS AT —33°.
(Smith, F. H.t 1917.)
Gm. Atoms Sodium Gm. Atoms Pb Gm. Atoms Na Gm. Atoms Pb
per Liter of Liquid Dissolved per Gm. per Liter of Liquid Dissolved per Gm.
Ammonia. Atom Na. Ammonia. Atom Na.
0.078 1-95 0.13 2.17
0.093 2-20 °-I4 2-12
0.094 2.03 0.33 1.83
o.no 2.24 0.34 1.73
0.12 1.78
LEAD ACETATE Pb(C2H3O2)2.3H2O.
loo gms. H2O dissolve 55.04 gms. Pb(C2H3O2)2 at 25°. (Jackson, 1914.)
EQUILIBRIUM IN THE SYSTEM LEAD OXIDE, ACETIC ACID, WATER AT 25°.
(Sakabe, 1914.)
Gms. per 100 Gms. Sat. Sol. „ .. . _. Gms. per 100 Gms. Sat. Sol.
(C2H302)(HO)Pb-f-
PbO.
CH3COOH.
•» oouu jrnase. . /
PbO.
CHjCOOI
4.18
2*-53
Pb(C2H302)2.3H20
>
3.80
16.78
«
7-I5
7.20
3.16
13.07
"
5.20
5-61
2.64
5-49
«
3-78
4.17
3-34
5-36
M
2.89
2-5i
4-38
7-30
«
i-45
1.03
5.18
7.92
" +(0,11302) (HO)Pb
i .05
0-54
5-59
7.72
(QHAXHOJPb
1.07
0.48
6.51
7-79
"
i
0.20
PbO
Equilibrium was attained quickly in the acid solutions but 2-3 days were required
in case of the basic salts. Both sat. solutions and solid phases were analyzed.
LEAD ACETATE 35O
EQUILIBRIUM IN THE SYSTEM LEAD ACETATE, LEAD OXIDE, WATER AT 25°.
(Jackson, 1914.)
^26 Of
Gms. per too Gms. Sat. Sol. Solid
djsof Gms. per ioo Gms. Sat. Sol. Solid
Sat. Sol.
' PbO.
Pb(C2H302)2.
Phase.
Sat. Sol.
PbO. Pb(C2H3Oo)2. Phase.
I .326
— 0
.27*
35-19
i-3
2
.280
24
•74
49
.21
3.1.3+1.2.4
1-334
'+0
.IO
35-60
«
2
.048
23
•59
43
•17
1.2.4
1.367
I
.OI
37-14
it
I
•951
22
.78
40
.78
((
1.422
3
.38
38.93
a
I
•657
19
-63
3i
.40
ii
1-531
6
.01
41-95
((
I
•599
18
•73
29
-63
tt
1.658
9
•47
44.71
(C
I
.382
14
.62
20
.96
tt
. . .
14
.22
47.88
((
I
.348
13
.41
19
-65
ft
1.852
14
-44
47.92
((
I
.229
10.66
12
•99
tt
. . .
15
.89
48.951
.3+3-1.3
I
.157
8
•47
8
.64
tt
1.930
IS
.90
48.42
3.1.3
I
.119
7
.87
5
•27
tt
1.942
16
•25
48.85
((
I
.117
7
•79
5
•25
ft
1.956
16
-65
49.04
((
4
•17
Pb(OH)2
2.024
18
-83
48.71
tt
I
.100
6
'•*4
4
•3i
n
2.161
22
•23
48.52
((
I
•095
6
•54
4
•25
tt
2.193
22
•94
48.96
ft
I
-085
5
.91
3
.82
tt
23
.28
49.14
ft
I
•075
5
.29
3
.40
tt
2.22O
23
•53
49.01
{(
o
.20
0
.11
<t
In this case the acidity is expressed in terms of PbO.
i.3 = Pb(C2H302)2.3H20, 3.1.3 = 3Pb(C2H302)2.Pb0.3H20, 1.2.4 «Pb(C,HA)r
2PbO.4H2O.
The above results show the solubility of lead acetate in aqueous solutions
containing increasing amounts of lead hydroxide. The mixtures were constantly
agitated for periods varying from 2 to 7 days. Both the saturated solutions and
the solid phases were analyzed. The basic lead in a given sample was determined
by measuring the volume of standard acid neutralized by it. The neutral lead
acetate was determined by precipitation of the lead as sulfate or as oxalate.
SOLUBILITY OF LEAD ACETATE IN AQ. SOLUTIONS OF POTASSIUM ACETATE AT 25°.
(Fox, 1909.)
Gms. per ioo Gms. Sat. Sol.
CHaCQOK. ' (CH3COO),Pb. Solid Phase.
o 35.9 (CH3COO)2Pb.3H20
13-87 38.05
15.40 36.90
SOLUBILITY OF LEAD ACETATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Wt.%^ ^of £ms-pb Wt-% ^ of H^'Pb
Solvent. So1' Sat. Sol. ' Solvent. SoL Sat. Sol.
o -343 36.5 (CaHaOa^Pb.sH-jO 70 0.955 12.4 (C2H3O2)2Pb.3H20
10 -275 32.3 80 0.907 9.4
20 .215 28.6 81 0.905 9
30 .157 25 " 85 0.855 4 (C2Ha02)2Pb
40 -105 21.9 90 0.826 1.6
50 .055 18.7 95 0.806 0.6
60 .002 15.6 ioo 0.790 0.4
ioo gms. 95% formic acid dissolve o.99(?) gm. Pb(C2H3O2)2 at 19.8°. (Aschan, 1913.)
ioo gms. anhydrous lanolin (m. pt.46°) dissolve i .1 gm. Pb(C2H3O2)2at45°. (Klose, '07.)
ioo gms. glycerol dissolve about 20 gms. Pb(C2H3O2)2 at 15°. (Ossendowski, 1907.)
LEAD ARSENATE PbHAsO4.
Two gm. portions of amorphous dilead arsenate were agitated at 32° with 90 to
1 80 cc. portions of 0.0338 normal aqueous ammonia for two days. The saturated
solutions were found to contain only traces of lead but amounts of As2O6 varying
from 1.956 to 1.429 gms. per liter. (McDonnell and Smith, 1916.)
351 LEAD BENZOATE
LEAD BENZOATE Pb(C7H6O2)2.H2O.
SOLUBILITY IN WATER.
(Pajetta, 1906.)
t°. 18°. 40.6°. 49°.
Cms. PbCCrHsC^ per 100 gms. sat. sol. 0.149 0.249 0.310
LEAD BORATE Pb(BO2)2.H2O.
100 cc. anhydrous hydrazine dissolve about 2 gms. Pb(BO2)2 at room temp.
(Welsh and Broderson,.i9is.)
LEAD BROMATE Pb(BrO3)2.H2O.
'b(BrO3)2 at K,
(Rammelsberg, 1841; Bottger, 1903.)
100 gms. water dissolve 1.32 gms. Pb(BrO3)2 at 19.94°.
(Rammelst
LEAD BROMIDE PbBr2.
SOLUBILITY IN WATER.
(Lichty — J. Am. Chem. Soc. 25, 474, '03.)
t°.
Density
of Solutions,
H2O at o°.
Gms. PbBr2 per too
Milligram Mols. PbBr2 per 100
cc. Solution. Gms. H2O.
cc. Solution.
Gms. H2O.
o
I .0043
0-4554
0-4554
1.242
1.242
15
1-0053
0.7285
0.7305
1.987
1.989
25
I .Oo6l
0.9701
0-9744
2.646
2.655
35
I -0060
I.3I24
1.3220
3-577
3-603
45
I .0059
I-7259
1-7457
4.705
4-760
55
I .0046
2 .IO24
2.1376
5-731
5.827
65
I .0028
2.516
2-574
6.859
7.016
So
I -OOOO
3-235
3-343
8.819
9.113
95
0-9995
4-1767
4-3613
11.386
11.890
100
4-550
4-751
12.40
12.94
SOLUBILITY OF LEAD BROMIDE IN AQUEOUS HYDROBROMIC ACID
AT IQ°.
100 grams H2O containing 72.0 grams HBr dissolve 55.0 grams
PbBr2 per 100 gms. solvent, and solution has Sp. Gr. 2.06.
(Ditte — Compt.rend 92, 719, '81.)
SOLUBILITY OF LEAD BROMIDE IN PYRIDINE.
(Heise, 1912.)
j.o Gms. PbBrz per c i-j -ni. *o Grns. PbBr2 per c IM -D^
100 Gms. Pyridine. Solld Phase" * ' 100 Gms. Pyridine. Solld Phase'
— 26 I. O2 PbBrz.aCsHjN 45 O.66l PbEr^CsHsN
— 10 0.89 " 64 0.800 "
- 5 0.84 " 77 0.969
o 0.80 95 1.33
+ 13 0.661 " loo 1.44 "
I9tr.pt. ... " +PbBr2.2C5H6N 105 1.56
26 0 . 583 PbBr2.2C5H6N
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES OF LEAD BROMIDE AND OTHER COMPOUNDS.
Lead Bromide + Lead Chloride (Monkemeyer, 1906.)
+ Lead Iodide
" + Lead Fluoride (Sandonnini, 1911.)
" + Lead Oxide (Sandonnini, 1914.)
-j- Mercuric Bromide (Sandonnini, 1912, 1914.)
" " -j- Silver Bromide (Matthes, 1911.)
LEAD BROMIDE
352
LEAD
LEAD
Dicyclohexyl DiBROMIDE (C6Hn)2PbBr2.
Dicyclohexyl DiCHLORIDE (C6Hn)2PbCl2.
SOLUBILITY OF EACH IN SEVERAL SOLVENTS AT 22.5°.
(Gruttner, 1914.)
Grams per 100 Grams Solvent.
Solvent.
Benzene
Carbon Tetrachloride
Chloroform
Alcohol + Pyridine (i : i)
O.OI4
O.OO4
0.078
2.560
(C6Hn)2PbCl2.
0.016
0.004
0.083
2.904
Similar results are also given for lead tetracyclohexyl, PbCCeHiOi, lead tetra-
phenyl, Pb(C6H8)4, and lead diphenyldicyclohexyl, Pb(C6H6)a(C6Hn)j.
Gms. per 100 Gms. Solvent.
Solvent.
Alcohol
Benzene
Carbon Tetrachloride
Ethyl Acetate
LEAD CAPROATE, CAPRYLATE, CAPRATE, etc.
SOLUBILITY OF EACH IN ETHER AND IN PETROLEUM ETHER.
(Neave, 1912.) /
Solubility in Ethyl Ether. Solubility in Pet. Ether.
Gms. Salt per 100 cc. Sat. Sol. Gms. Salt per 100 cc. Sat. Sol.
Pb(C6Hn)4.
Pb(C6H5)4.
Pb(C6H6)2(C6H11)2.
O.OIO
O.O2O
0.324
1.068
I-I45
2.298
0.244
0.303
0.845
0.030
0.123
0.231
Pb
«
a
tt
tt
n
n
(i
tt
Caproate
Heptylate
Caprylate
Nonylate
Caprate
Myristate
Laurate
Palmitate
Stearate
73-74
90.5-91.
83.5-84-
94-95
IOO
107
103-104
112
125
At 20°. At B. pt. of Sat. Sol. At 20°. At B. pt. of Sat. Sol.
i . 364 ... o . 0608
5 0.2397 1.490 0.020 0.0528
5 0.0938 0.546 practically insol. 0.0384
0.1115 0.2404 0.0450
0.0290 0.4285 0.0170
practically insol. 0.0555 0.0210
" 0.0205 " practically insol.
0.0261
practically insol. " 0.0170
The ethyl ether was distilled over sodium. Petroleum ether distilling between
4O°-6o° was used. The solutions were stirred constantly at 20°. A definite volume
of the sat. solution was evaporated to dry ness and residue weighed in each case.
LEAD CARBONATE PbCO3.
SOLUBILITY IN WATER BY ELECTRICAL CONDUCTIVITY METHOD.
(Kohlrausch and Rose, 1893; Bottger, 1903.)
I liter of water dissolves 0.0011—0.0017 gni- PbCO3 at 20°.
SOLUBILITY OF LEAD CARBONATE (NEUTRAL) IN AQUEOUS SOLUTIONS OF
CARBON DIOXIDE AT 18°.
(Pleissner, 1907.)
Millimols per Liter. Milligrams per Liter.
CO2.
o
0.064
0.123
0.328
0.592
0.988
2.40
o
2.8
5-4
14.4
26
43-5
106
Pbc3.
1.75
6
7
8.2
0.008
0.029
0.034
0.040
0.048 2 9.9
0.053 43-5 10.9
0.076 106 15.4
A determination of the solubility of basic lead carbonate in water gave 1.6 mg.
Pb3(CO3)2(OH)2 per liter = 1.3 mg. Pb or 0.006 millimol Pb.
353 LEAD CARBONATE
Data for equilibrium in the system composed of K2COs + PbCO3 + K2CrO4
+ PbCrO4 at 25° are given by Goldblum and Stoffella, 1910.
Data for equilibrium by lead carbonate precipitation in aq. solutions of sodium
salts at 25° are given by Herz, 1911.
LEAD CHLORATE Pb(ClO3)2.H2O.
100 grams H2O dissolve 151.3 gms. Pb(QO3)2, or 100 gms. sat. solution con-
tain 60.2 gms. Pb(ClO3)2 at 18°. Density of solution, 1.947. (Mylius and Funk, 1897.)
100 gms. H2O dissolve 440 gms. Pb(ClO3)2 at 18°, dn = 1.63. (Carlson, 1910.)
LEAD CHLORIDE PbCl3.
SOLUBILITY IN WATER. (Lichty; see also Formanek, 1887; Bell, 1867; Ditte, 1881.)
to
Density
Gms. PbCl2
per 100
Milligram Mols.
PbCl2 per TOO
.
of Solutions,
H2O at o°.
cc. Solution.
Gms. H2O.
cc. Solution.
Grams H2O."
0
I .0066
0.6728
0.6728
2.421
2.421
15
1.0069
0.9070
0.9090
3 -265
3.272
25
1.0072
I .0786
I .0842
3.882
3-903
35
I .0060
i -3*50
1.3244
4-733
4-767
45
I .OO42
1.5498
I-5673
5-579
5-644
55
I .0020
1.8019
1.8263
6.486
6-573
65
0-9993
2.0810
2.1265
7-490
7-65I
80
0.9947
2.5420
2.6224
9.150
9-439
95
0.9894
3-0358
3-I654
10-926
n-394
100
3.208
3-342
11.52
12 .01
SOLUBILITY
OF LEAD
CHLORIDE IN
AQUEOUS 'SOLUTIONS OF
ACETIC ACID
AT 25°.
(Hill, 1917.)
Normality
Dissolved PbCl2.
Normality
Dissolved PbCl2.
of Acetic
Gms.
Equiv.
of Acetic
Gms.
Equiv.
Acid.
per Liter.
per Liter.
Acid.
per Liter.
per Liter.
O
10.77
0-07753
0.465
IO.27
0.07392
0.05
10.82
0.07782
0.929
9-45
o . 06803
O.IO
10.85
0.07717
1.845
7.90
o.os686
O.2O
10.70
0.07703
3-680
5.26
0.03788
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS AMMONIUM CHLORIDE AT 22°.
(Bronsted, 1911.)
Gm. Equivalents per Liter. Gm. Equivalents per Liter.
' NH.C1. ' Pbd.. ' SoMPhaSe' 'NH.C!. ' PbCl.. ***»"•
O 0.0749 PbCl, 0.8 0.0087
o.i 0.0325 " i 0.0080 "
0.2 0.0194 1.5 0.0073
0.4 0.0138 2.5 0.0092
0.5 0.0130 " 4 0.0182 "
0.52 0.0127 " +NH«a.2PbCl1 6 0.0473
0.55 0.0123 NH4Cl.2PbCl2 7.29 0 . 0898 "• +NH4C1
0.65 0.0105 " 7.29 O NHiCl
For additional results at 25.2° see von Ende, 1901.
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID.
Results at l8°. (Pleissner, 1907.) Results at 25.2°. (von Ende, 1901.)
Normality Gms. PbClj Normality Millimols Normality Millimols
ofHCl. per Liter. of HC1. PbCl2 per Liter, of HC1. PbCl, per Liter.
o 9-34 o 38.8 . 1.026 4.41
o.oooi 9-305 0.0045 37-35 2.051 5.18
0.0002 9.300 O.OI5I 33.75 3.085 7.78
0.0005 9-243 0.0452 25.46 5 19.38
0.00102 9.200 0.1850 10.25 7-5 65.86
0.0102 8.504 0.5142 5.37 12.05 164.30
LEAD CHLORIDE 354
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OP HYDRO-
CHLORIC ACID.
(At o°, Engel — Ann. chim. phys. [6] 17, 359, '89; at 25°, Noyes — Z. physik. Chem. 9, 623, '92; at differ-
ent temperatures, Ditte — Compt. rend. 92, 718, '81; see also Bell — J. Chem. Soc. 21, 350, '68.)
Cms. HC1
Liter.
Cms. PbCl2 per
Liter at:
Cms. HC1
per 100
Cms. H2O.
Cms. PbCl2 per 100 Gms. Solution at:
0°.
25°.
o0.'"
20°.
40°.
55°.
80°.
0
3-83
10
•79
O
8.0
II .
8
17.0
21 .
0
31.0
o-5
4-5
9
• O
100
1.2
I.
4
3-2
5
5
12.0
1.0
3-6
7
.6
J5o
i-5
2.
o
5-o
7
,5
16.0
2.0
2.2
6
.0
200
3-5
5-
o
8.2
ii
•7
21-5
3-o
1.6
5
.0
250
6-5
8.
0
13.0
16
,2
28.5
6
1.4
3
.1
300
10.7
12.
5
17-5
22
.0
3S-o
10
I .2
i
.8
400
21-5
24.
0
...
• •
• .
...
100
1.2
2OO
5-2
.
..
250
10-5
•
300
17-5
.
400
40-0
.
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SALT SOLUTIONS
AT 25°.
(Noyes; in HgCl2 solutions at 20°, Formanek — Chem. Centralb. 270, '87.)
In Aqueous Solutions of:
HCl, KC1, MgCl2, CaCl2, MnCl2 In CdCl2
and ZnCl2 Gram Equivalents Gram Equiv.
per Liter of: per Liter.
In HgCl2
Gram Equiv.
per Liter.
InPb(N03)2
Gram Equiv.
per Liter.
'Salt. PbCl2. CdG2. PbCl2.
o.o 0.0777 °-°° 0.0777
0.05 0.050 0.05 0.0601
o.io 0.035 0<I° 0.0481
0-20 0-021 0-20 0.0355
HgCl2. PbCl2.
o.o 0.0777
o.i 0.0992
Pb(N03)2. PbCl2.
o.o 0.0777
O-2 0.0832
The above results were calculated to grams per liter plotted on cross-
section paper, and the figures in the following table read from the
curves.
Gms.
Salt
Grams PbCl2 per Liter in Aqueous Solutions of:
per
Liter.
HCl.
KC1.
MgCl2.
CaCl2.
MnCl2.
ZnCl2.
CdCl2.
HgCl2. Pb(N03)a
o
I
10.79
8-5
10.79
9-3
10.79
7-7
10.79
8.7
10.79
9-5
10.79
10.79
10.2
io-79(
II .0
N) 9-7i(F)
9.8
10.79
10.8
2
6-5
8.2
6-5
7.6
8-3
. . .
9-7
11.4
IO.O
10.85
3
5-2
7-2
5-7
6.7
7-3
9.2
11,7
10.3
10.87
4
4-3
6-5
5-2
6.0
6-3
• • •
8.6
12.0
10.5
10.90
6
3-2
5-3
4.4
4.8
5-°
...
7-7
12.7
II. O
10.95
8
4-5
3-9
4.1
. ..
7.0
13-3
ii. 6
II .00
10
2.1
3-9
3-3
3-5
. . ,
6-3
14.0
12.2
11.05
14
2.8
3-o
5-4
I3.2
11.15
20
14.8
1 1 . 20
40
IQ-0
11.70
355
LEAD CHLORIDE
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OF LEAD NITRATE AT 25°.
Results by Harkins, 1911. Results by Armstrong and Eyre, 1913.
Gms. per Liter Sat. Sol.
dmm of Sat.
V Sol.
Pb(N03)2. PbCl2.
o 10. 81
I . 0069
3.31 10.67
1.0095
8.28 10.65
I.OI39
16.56 10.84
I. 02 10
33-12 11.57
...
Aq. Pb(N03)2
Sol., Gms. per
1000 Gms. H2O.
Gms. PbCU per
1000 Gms.
Sat. Sol.
0
10.89
3-31
10.96
6.62
i°-53
33-12
11.15
82.80
12.95
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AT 25.2°. (von Ende, 1901.)
Normality
of KC1.
0
0.001
Gm. Equiv. PbClj
per Liter.
0.07760
0.07664
0.0025
0.07570
0.0049
O.OO99
0.0200
0.07404
0.07056
0.06432
0.0599
0.04524
Normality
Gm. Equiv. PbCl2
of KC1.
per Liter.
0.0999
0.02380
0.5006
0.01480
0.7018
0.01476
0.9991
o . 00980
I.50I8
0.00996
2.OO24
O.OIII2
3.0036
0.01948
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AT 20°. (Bronsted, 1912.)
Gm. Equivalents per
1000 Gms. Solution.
"KC1.
O.IQ5
PbCl2.
0.01900
0.299
0.01452
0-375
0.483
0.01324
0.01236
0.510
0-575
0-639
0.0125
0.01068
0.00954
0.930
I .224
1-575
1.884
0.00770
0.00736
0.00786
0.00894
Solid Phase.
Gm. Equivalents per
1000 Gms. Solution.
Solid Phase.
PbCl2
KC1.
2.10
2. 2O
2.29
2.36
+2PbCl2.KCl
aPbCVKCl
2.45
2.66
2.77
2.91
3-05
2PbCl2.KCl
2PbCl2.KCl+PbCl2.KCl.|H2O
PbCl,.KCl.JH20
PbCl2.
0.01022
O.OIO6O
O.OII84
O.OI3OO
0.01308
0.01396 '
0.01476
0.01550
0.01656
0.01780
4.57* 0.0280*
Gm. equivalents per 1000 Gms. H^O.
Data for the solubility of lead chloride in aqueous KC1 and aqueous NaCl are
given by Demassieux, 1914.
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OF ALCOHOL AND OF
MANNITOL AT 25°. (Kernot and Pomilio, 1912.)
Results for Aqueous Ethyl Alcohol. Results for Aqueous Mannitol.
+KC1
Gms. per Liter .Solution.
C2H5OH.
5.75
11.51
23.02
46.05
92.10
184.20
10
PbCl2.
IO-75
16
9.36
9.14
8.25
7.12
4.76
Gms. per Liter Solution.
(CH2OH)2(CHOH)T
PbCl2.
IO-75
10.42
10.67
10.64
10.91
ii. 16
11.29
SOLUBILITY OF LEAD CHLORIDE IN GLYCEROL. (Presse, 1874.)
I part glycerol + 7 parts H2O dissolve 0.91 per cent PbCl2.
I part glycerol + 3 parts H2O dissolve 1.04 per cent PbCl2.
I part glycerol + i part H2O dissolves 1.32 per cent PbCl2.
Pure glycerol dissolves 2 per cent PbCl2.
2.84
5.69
11.38
22.76
45.53
91.06
LEAD CHLORIDE
356
SOLUBILITY OF LEAD CHLORIDE IN AQUEOUS SOLUTIONS OF SEVERAL
COMPOUNDS AT 25°. (Armstrong and Eyre, 1913.)
Gms. PbCl2
Gms. PbCl2
Aqueous
Solution of:
per 1000
Gms. H2O.
per 1000
Gms. Sat.
Sol.
Aqueous
Solution of:
Gms. C^mpd.
per 1000
Gms. H2O.
per 1000
Gms. Sat.
Sol.
Water alone
0
10.89
Ethyl Alcohol
11.51
10.43
Glycol
15.51
10-75
Glycerol
23.01
10.98
tt
62.04
10.90
Propyl Alcohol
I5.OI
10.08
Acetaldehyde
II.OI
10.54
a it
60.06
9-37
"
33-03
9.82
Methyl Acetanilide
29.82
10.25
Paraldehyde
II.OI
10.50
Hydrochloric Acid
9-12
4-23
u
33-02
9.96
n it
18.23
3.60
ioo cc." anhydrous hydrazine dissolve 3 gms. PbCl2 at ord. temp, with decom-
position. (Welsh and Broderson, 1915.)
SOLUBILITY OF LEAD CHLORIDE IN PYRIDINE. (Heise, 1912.)
to
Gms. PbCljs
per ioo Gms.
Solid Phase.
Pyridine.
— 20
0.303
PbCl2.2C5H5N
0
0.364
tt
+ 22
0-459
n
44
0-559
11
65
0.758
tt
76
90
94
IO2
Gms. PbCl2
per ioo Gms.
Pyridine.
0.893
1.07
I. 12
Solid Phase.
PbCl2.2C5H5N
it
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR
THE FOLLOWING MIXTURES OF LEAD CHLORIDE AND OTHER COMPOUNDS.
Lead Chloride + Lead Fluoride
+ Lead Iodide
+ Lead Oxide
-j- Lead Sulfide
+ Lithium Chloride
+ Magnesium Chloride
+ Manganese Chloride
-j- Potassium Chloride
-J- Rubidium Chloride
+ Silver Chloride
-f Strontium Chloride
-j- Sodium Chloride
-j- Thallium Chloride
-j- Tin Chloride
(Sandonnini, 1911.)
(Monkemeyer, 1906.)
(Ruer, 1906.)
(Truthe, 1912.)
(Tries, 1914.)
(Menge, 1911.)
(Sandonnini, 1911, 1914.)
(Tries, 1914; Lorenz and Ruckstuhl, 1906.)
(Matthes, 1911; Tries, 1914.)
(Sandonnini, 1911, 1914.)
(Tries, 1914-)
(Korreng, 1914; Sandonnini, 1913.)
(Hermann, 1911; Sandonnini, 1911, 1914.)
(Herrmann, 1911.)
+ Zinc Chloride
LEAD CHLORIDE (Basic).
SOLUBILITY OF BASIC LEAD CHLORIDES IN WATER AT 18
(Pleissner, 1907.)
Compound
Basic Lead Chloride
Formula.
Gms. per Liter Sat. Aq.
Solution.
Pb
0.079
0.021
Pb Salt.
0.099
0.025
PbCl2.PbO.H2O
J " PbCl2.3PbO.H2O
LEAD FluoroCHLORIDE PbFCl.
SOLUBILITY OF LEAD FLUOROCHLORIDE IN WATER AND IN AQUEOUS SOLUTIONS.
(Stark, 1911.)
Solubility in Water. Solubility in Aq. Solutions at 25°.
t.
Gms. PbFCl
per ioo Gms.
A,.So,u,ion G-£FC>
H,0.
Ot:
Sat. Sol.
0
0.02II
o . 00996 n PbCl2
0.0030
18
0.0325
0.0195 n
O.OOOS
25
0.0370
0.0392 n "
0.0005
IOO
O.IOSI
Aq. Solution
of:
Gms. PbFCl
per ioo cc.
Sat. Sol.
o.o535wHCl 0.0758
0.1069^ " 0.1006
0.0518 n CH3COOH 0.0512
O.I055/J
0.0561
357 LEAD CHROMATE
LEAD CHROMATE PbCrO4.
SOLUBILITY OF LEAD CHROMATE IN WATER.
t°. "* G™rffi°' Method. Authority.
Normality
Milligrams *
'b per 100 cc. b;
it. SQL at:
Normality
of HC1.
18°.
25°-
37°.
HNOj.
O.I
3.86
4.96
7.40
O.I
0.2
8-15
10. 06
15.40
0.2
o-3
I3-56
I7-38
27.30
°-3
0.4
22.14
27.78
43.60
0.4
0.5
32.30
42.60
68
o-5
0.6
46.60
61.06
97.20
0.6
l8 3.0.IO"7 O.OOOIO Solution equilibrium (Beck and Stegmiiller, 1910.)
1 .4. 1 0~7 0 . 00004 (Auerbach and Pick.)
1 8 3.2.IO"7 O.OOOIO Conductivity (Kohlrausch, 1908.)
20 2.I.IO"7 0.00007 Radio Indicators (v. Hevesy and Rona, 1915.)
SOLUBILITY OF LEAD CHROMATE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
AND OF NITRIC ACIDS. (Beck and StegmiUler, 1910, 1911.)
Solubility in Aq. HC1. Solubility in Aq. HNO3 at 18°.
Milligrams Pb per
100 oc. Sat. Sol.
2; 67
4.70
6.46
8.3I
10.31
12.39
Results are also given for the solubility of mixtures of lead chromate and
lead sulfate in aqueous hydrochloric acid at 25° and 37°.
SOLUBILITY OF LEAD CHROMATE IN AQUEOUS POTASSIUM HYDROXIDE SOLUTIONS.
(Lacland and Lepierre, 1891.)
t°. Grams KOH per loo cc. Grams PbCrO4 per icocc.
15 2.308 I.Ip
60 2.308 1.62
80 2.308 2.61
102 2.308 3.85
LEAD CITRATE Pb(C6H5O7)2.H2O.
SOLUBILITY IN WATER AND IN ALCOHOL.
100 gms. H2O dissolve 0.04201 gm. Pb(C6H5O7)2.H2O at 18°, and
0.05344 gm. at 25°.
100 gms. alcohol (95%) dissolve 0.0156 gm. Pb(C6H6O7)2.H2O at
1 8°, and 0.0167 gm- at 25°- (Partheil and Httbner — Archiv. Pharm. 241, 413, '03.)
LEAD DOUBLE CYANIDES.
SOLUBILITY IN WATER.
(Schuler — Sitzber. Akad. Wiss. Wien, 79, 302, '79.)
Double Salt. Formula. t°. ^^Q00
Lead Cobalticyanide Pbg[Co(CN)6]2.7H2O 18 56.5
Lead Cobalticyanide PbJCo(CN)6]2.7H2O 19 61.3
Lead Potassium Cobalticyanide PbKCo(CN)6.3H2O 18 14.8
Lead Cobalticyanide Nitrate Pb3fCo(CN)6]2.Pb(NO3)2.i2H2O 18 5.9
Lead Ferricyanide Nitrate PbjFe(CN)6]2.Pb(NO3)2.i2H2O 16 7.5
Lead Potassium Ferricyanide PbKFe(CN)6.3H2O 16 21.0
LEAD FLUORIDE PbF2.
One liter of water dissolves 0.6 gm. PbF2 at 9°, 0.64 gm. at 18°, and O.68 gm. at
26.6° (conductivity method). (Kohlrausch, 1908.)
ipo cc anhydrous hydrazine dissolve 6 gms. PbF2 at room temp, with decom-
position. (Welsh and Broderson, 1915,)
Freezing-point data (solubility, see footnote, see p. i) for mixtures of PbF2 and
PbI2 are given by Sandonnini (1911); for mixtures of PbF2 + PbO by Sandon-
nini (1914); for mixtures of PbF2 + Pb3(PO4)2 by Amadari (1912), and for
PbF2 + NaF by Puchin and Baskow (1913).
LEAD FORMATE
358
LEAD FORMATE Pb(HCOO)2.
SOLUBILITY OF LEAD FORMATE IN AQUEOUS SOLUTIONS OF BARIUM FORMATE AT 25°.
(Fock, 1897-)
Mol. % in Solution.
Grams per Liter.
Sp. Gr. of
In Solid Phase Mol. % of
Pb(HCO2)2.
Ba(HCO2)2.
' Pb(HC02)2.
Ba(HCO2)2.
Solutions.
Pb(HCO2)2.
Ba(HC02)2.'
O
IOO
28.54
1.2204
0
IOO
0.2Q
99.71
I .IO4
28.65
I.22I3
1.72
98.28
0.74
99.26
2.803
28.90
I .2251
5-29
94.71
1.24
98.76
5-3°9
32.24
1.2529
11.94
88.06
2.91
97.09
ii .42
29.29
I.234I
24.81
75-19
5-92
94.08
23.11
28.13
1-2355
56.54
43-46
IOO
0
28.35
I .0911
IOO
0
LEAD HYDROXIDE Pb(OH)2.
SOLUBILITY OF LEAD HYDROXIDE IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE.
(Moist Lead Hydroxide used, temperature not given.)
(Rubenbauer, 1902.)
Grams per 100 cc. Solution.
Amount of Na
Amt. of Pb
Mol. Dilution
in 20 cc.
in 20 cc.
of NaOH.
o . 2024
O.IOI2
2.27
0.3196
0.1736
1.44
0.5866
0-3532
0.785
0.9476
o . 407 i
0.485
1.7802
0.5170
0.258
NaOH.
1-759
2.778
5-1°
8-235
I5-470
Pb(OH)2.
0.590
I .OIO
2.056
2.370
3.010
LEAD IODATE Pb(IO3)2.
One liter of water dissolves 0.0134 gm. Pb(IO3)2 at 9.2°, 0.019 gm. at 18° and
O.023 gm. at 25.8°. (Kohlrausch, 1908; Bottger, 1903.)
One liter H2O dissolves 0.0307 gm. Pb(IO3)2 at 25°. (Harkins and Winninghoff, 1911.)
SOLUBILITY OF LEAD IODATE IN AQUEOUS SALT SOLUTIONS AT 25°.
(H. and W., 1911 )
Gms. per Liter.
KNO3.
0.202
I .Oil
5-055
20.220
Gms. per Liter.
Gms. per Liter.
Pb(I03)2.
0.0318
0.0363
0.0567
0.0708
LEAD IODIDE PbL
o
15
25
35
45
55
65
80
95
IOO
Density.
(H2O at o°.)
I. 0006
0.9998
o . 9980
0.9951
0.9915
0.9872
0-9745
o 9671
KIO3.
O.OII3
0.0227
Pb(N03)2.
0.0165
0.165
SOLUBILITY
(Lichty,
Grams PbI2
Pb(IO3)2.
0.0199
0.0122
0.0242
O.OII5
IN WATER.
1903.)
per 100.
cc. Solution.
O.O442
0.0613
0.0762
0.1035
o . 1440
0.1726
0.2140
0.2937
0.3814
O.42O
Grams H,O.
0.0442
O.O6I3
0.0764
0.1042
0-1453
0.1755
0.2183
0.3023
0.3960
0.436
Pb(N03)2.
1.656
16.561
82.805
496.83
Pb(I03)2.
O.OO52
0.0045
0.0078
0.0418
Millimols PbI2 per 100.
cc. Solution.
0.096
0.133
0.165
0.224
0.312
0-374
0.464
0.637
0.828
0.895
Grams H2O.
0.096
0.133
0.166
0.226
0-315
0.381
0-473
0.656
0.859
0.927
^ Data for the solubility of lead iodide in water by the conductivity method are
given by Bottger, 1903; Kohlrausch, 1904-05; Denham, 1917.
359 LEAD IODIDE
SOLUBILITY OF MIXTURES OF LEAD IODIDE AND POTASSIUM IODIDE IN WATER.
(Ditte, 1881; Schreinemakers, 1892.)
Gms. per 1000 Gms. H2O.
PbI2. KT
5 ... 163 Double Salt +PbI2 50 526.7 1906 Double Salt +KI
20 9 260 64 789.3 2161
28 25 325 83.5 1,108.6 2434
39 45 449 92 1,273 2566
67 255 751 137 2,382 3278
80 731 1186 165 4,187 4227
80 569.9 976.4 218 10,303
104.5 1411 1521 241 12,803 7998 "
120 2151 1812 " 242 12,749 ... "
137 2874 2097 250 15,264
175 5603 2947 157 5, 218 gms. Pbl,.2Kl >bl2.2Kl.2iHso
189 ... 3339 " 172 6,489 '
9 96.6 1352 ' +KI 186 7,903
13 114.3 1384 " 194 9,266 '
23 186.3 I3I° " 201 11,320 '
Ordinary solubility method used for temperatures below boiling-point of the
solution and sealed tube (with constriction in middle) method used for tem-
peratures above boiling point.
One liter sat. aqueous solution of iodine dissolves 0.0021 6 gm. mols. PbI2 (0.996
gms.) at 2O°. (Fedotieff, 1911-12.)
SOLUBILITY OF LEAD IODIDE IN ACETONE, ANILINE AND AMYL ALCOHOL.
(von Laszczynski, 1894.)
AO Gms. PbL per ioo
Gms. Solvent.
59 0.02
13 °-5o
184 i. 10
C5H7OH 133.5 0-02
SOLUBILITY OF LEAD IODIDE IN PYRIDINE.
(Heise, 1912.)
Gms. PbI2 Gms. Pbl,
t°. per ioo Gms. Solid Phase. t°. periopGms. Solid Phase.
Pyridine. Pyridine.
— 43 . 5 f .-pt. ... Pblj.sCjHjN 35 O.l88 Pblj^CsHjN
—37 0.166 " 57 0.190
— 20 0.175 " 77 0.228 " •
— 9 0.186 " 92 0.200 "
o 0.200 " 98 0.340 "
+ 3 0.215 " 105 0.370
6tr.pt. 0.225 Pbiz.aCjHsN+Pbiz^CsH^ 108 0.410 "
15 O.2O8 Pblz^CsHsN 112 0.445 "
ioo gms. 95% formic acid dissolve 0.25 gm. PbI2 at 19.8°. (Aschan, 1913.)
ioo cc. anhydrous hydrazine dissolve 2 gms. PbI2 at room temp, with decom-
position. (Welsh and Broderson, 1915.)
Freezing-point data for mixtures of lead iodide and silver iodide are given
by Matthes (1911).
T.F.AD MAT.ATE Pb.C4H4O5.3H2O.
SOLUBILITY IN WATER AND ALCOHOL.
(Partheil and Hubner, 1903.)
ioo gms. H2O dissolve 0.0288 gm. PbC4H4Os.3H2O at 18°, and 0.06504 gm. at
25°.
ioo gms. 95% alcohol dissolve 0.0048 gm. PbC4H4O6.3H2O at i8°-25°.
Density of alcohol employed = 0.8092.
LEAD LAURATE 360
LEAD LAUEATE, MYRISTATE, PALMITATE and STEARATE.
SOLUBILITY OF EACH IN SEVERAL SOLVENTS.
(Jacobson and Holmes, 1916.)
(See Lithium Laurate, p. 375, for formulas and other details. See also p. 362.)
Solvent.
Cms. of Each Salt (Determined Separately) per too Gms.
Solvent.
Pb Laurate.
Pb Myristate.
Pb Palmitate.
Pb Stearate.
35
O.OOQ
0.005
O.OO5
0.005
So
0.007
0.006
0.007
0.006
25
O.OOg
O.OO4
0
O
35
0.032
O.OO4
O.OOI
O.OOI
5°
0.264
0.052
0.012
0.004
15-5
0.061
0.056
0.051
0.039
25
0.096
0.078
0.069
0.051
35
0.113
0.082
0.076
0.062
5<>
0.280
O.II9
0.093
0.083
14-5
O.OIO
0.013
O.OIO
0.007
14
0.017
O.OIO
0.009
0.007
35-5
0.035
0.015
0.009
0.008
50
O.2OI
0.077
0.033
O.O2O
15
O.OII
O.OIO
0.009
0.008
Water
Abs. Ethyl Alcohol
u u <(
tt tt ((
Methyl Alcohol
Ether
Ethyl Acetate
(t u
tt tt
Benzene
LEAD NITRATE Pb(NO8)2.
SOLUBILITY IN WATER.
(Mulder; Kremers, 1854; at 15°, Michel and Kraft, 1854; at 17°, Euler, 1904.)
Grams Pb(N03)2 per 100 Gms. Grams Pb(NO3)2 per 100 Gms.
V .
O
10
17
20
25
30
Water.
Solution.
27.33^)
3L6
34-2
35.2
36.9
38.8
Water.
Solution.
41.9
45
47-8
52.7
57-1
34-54
36
44
50
52
56
60
•4
•3
•4
•7
L> 38. 8 W
48.3
54
56.5
60.6
66
40
50
60
80
IOO
17
69
78
88
107
127
52
•4
•7
.6
.76*
75
85
95
138.8
* Euler.
(i) Mulder, (2) Kremers, (3) Average of M and K.
Density of saturated solution at 17° = 1.405.
loo gms. H2O dissolve 55.8 gms. Pb(NO3)2 at 20°.
Pb(
(Euler.)
F(LeBlanc and Noyes, 1890.)
b(NO3)2 + KNO3 at 20° dissolve 95.39 gms. Pb(NO3)2.
+61.05 gniS. KNO3. (LeBlanc and Noyes, 1890.)
loo gms. H2O sat. with Pb(NO3)2 -f NaNO3 at 20° dissolve 38.42 gms. Pb(NO3)2
+84.59 Sms- NaNO3. (Le Blanc and Noyes, 1890.)
SOLUBILITY OF LEAD NITRATE IN AQUEOUS SOLUTIONS OF COPPER NITRATE
AT 20°.
Fedotieff, 1911-12.)
Gms. per 100 Gms. H2O.
0
-55 -ii2 J
1 OttL. O
.419
7-7
39-34
•354
15.04
27.80 ]
.322
24.63
19.05 i
.321
33-25
14.70
•343
Cu(NO3)o.
Pb(NO3)2."
1*20 ui 00.1. hjvsi.
37.96
13.08
1.360
60.32
8.19
I.45I
83.11
5-37
1.546
100.29
3-53
1.622
127.70*
2.33*
1.700
* Solid phase in contact with this solution = Pb(NO,), + Cu(NO,)2.6H,O.
361
LEAD NITRATE
SOLUBILITY OF LEAD NITRATE IN CONCENTRATED AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND VICE VERSA, DETERMINED BY SYNTHETIC METHOD.
(Isaac, 1908.)
(The several mixtures were enclosed in sealed tubes and lieated until only
one or two very small crystals remained undissolved. The temperature was
then determined at which the edges of these crystals just showed a change from
sharp to round or vice versa.)
Results for Lead Nitrate as
Solid Phase.
Cms, per 100 Cms. Sat. Sol.
Results for Sodium Nitrate as
Solid Phase.
t° Of
Saturation.
32
35-5
39-5
44
49.1
55
58
62
65
SOLUBILITY OF MIXED CRYSTALS OF LEAD NITRATE AND_STRONTIUM NITRATE
IN WATER AT 25°.
(Fock, 1897-)
' NaNO3.
Pb(N03)2.
34-42
19.69
34-15
20.33
33-71
21-35
33-35
22. 19
32-94
23.15
32.60
23-93
32.47
24.24
32-33
24-57
32.19
24-89
t° of
Saturation.
21
26.5
3i
38.8
41
44.25
51
Cms, per 100 Gms. Sat. Sol.
NaNOj.
Pb(NOa)2."
40.97
13.62
42.04
13.38
43-18
12.88
44.63
12.78
45 -11
12.94
46.03
12-45
47.28
12.50
49-03
11.76
49.92
11.56
Mol. per cent in Solution.
Gms. per ioo cc. Solution.
Pb(NO3)2.
Sr(N03)2.
Pb(N03)2.
SrCNO-O,.
IOO
0
46-31
O
87.41
12.39
50-47
4.56
78.68
21.32
53-92
8.14
56.39
43-61
45-34
17.81
60.29
39-71
44.48
18.74
33-70
36.30
25-23
35.03
24.58
75-42
19-13
37-54
o
IOO
o
71.04
Sp. Gr. of
Solutions.
.4472
.4336
.4288
,4263
4245
.4468
.4867
.5141
Mol. per cent in Solid Phase.
' PKNO^. * Sr(NO»)j. "
ioo
99-05
98.11
97.02
96.06
83-84
32.88
o
o
0.95
1.89
2.98
3.94
16.16
67.12
ioo
SOLUBILITY OF LEAD NITRATE IN ETHYL AND METHYL ALCOHOL.
Solvent.
Gms. Pb(NOj)2 per ioo Gms. Solvent at:
.
Aq. C2H5OH (Sp. Gr. 0.9282) 4.96
Abs. C2H5OH
Abs. CHsOH
50°.
14.9 (G)
(deB)
8°. 22°. 40°.
5.82 8.77 12.
0.04(20.5°)
1.37 "
(Gerardin, 1865; de Bruyn, 1892.)
ioo cc. anhydrous hydrazine dissolve 52 gms. lead nitrate at room temper-
ature with formation of a yellow precipitate. (Wekh and Broderson, 1915.)
SOLUBILITY OF LEAD NITRATE IN PYRIDINE.
(Walton and Judd, 1911.)
Gms. Pb(NO,)2
t°. per ioo Gms.
Solid Phase.
Pyridine.
-19.4
2-93 Pfc
.(NQ^C.H
-14-5
2.14
"
•IO
1.90
"
o
3-54
"
5.4
3-93
M
8.7
5-39
M
14.72
6.13
(«
19.97
6.78
"
24.75
8.56
•
30.03
10.96
M
34.97
13.20
«
40.03
16 94
«
Gms. Pb(NOj)
t°.
per ioo Gms.
Pyridine.
45
22.03
49-97
29-37
51 tr. pt.
59-52
36.70
70
47.29
80
61.60
89-93
90.21
94 94
128.06
96 tr. pt.
.
99.89
143-36
104.90
152
109.90
163.80
Solid Phase.
+Pb(NO,)2.3CsHlN
+3Pb(N03)1.2C6HlN
3Pb(NO,),.2C»H|N
LEAD NITRATE 362
SOLUBILITY OF LEAD NITRATE-NITRITE, Pb(NO3)2.Pb(NO2)2.2Pb(OH)2.2H2O,
IN AQUEOUS SOLUTIONS OF ACETIC ACID AT 13.3°.
(Chilesotti, 1908.)
Normality of Gms. PbO per 100 Normality of Cms. PbO per 100 cc.
Acetic Acid cc. Sat. Sol. Acetic Acid. Sat. Sol.
o 0.601 0.25 5-45°
0.0$ 1.323 0.50 9.690
o.io 2.185 °-75 IJ5-874
LEAD OXALATE PbC2O4.
One liter of water dissolves 0.0015 gni. PbC2O4 at 18° (conductivity
method). (Bottger — Z.physik. Chem. 46, 602, '03; Kohlrausch — Ibid. 50, 356, W-'os.)
LEAD OXIDES. SOLUBILITY IN WATER.
(Bottger; Ruer — Z. anorg. Chem. 50, 273, '06.)
No. Description of Oxide. G£r!S' pe?LUer.
1. Yellow Oxide, by boiling Pb hydroxide with 10% NaOH i . 03 X io~* o. 023
2. Red Oxide, by boiling Pb hydroxide with cone. NaOH 0.56X10"* 0.012
3. Yellow Oxide, by heating No. i to 630° 1.05X10"* 0.023
4. Yellow Oxide, by heating No. 2 to 740° 1.00X10"* 0.022
5. Yellow Oxide, by heating com. yellow brown oxide to 620° i . 09 X io~* o. 024
6. Yellow Brown Oxide commercially pure i.ioXio"* 0.024
7. Yellow Brown Oxide, by long rubbing of No. 5. i. 12X10"* 0.025
Bottger gives for three samples of lead oxide, 0.017, 0.021, and 0.013
gm. per liter respectively.
One liter H2O dissolves 0.068 gm. PbO at 18°, solid phase PbO and 0.1005 Sm-
PbO at 1 8°, solid phase Pb3O2(OH)2. (Pleissner, 1907.)
Results for the solubility of hydrated lead oxide in water and dilute H2SO4
solutions are given by Sehnal (1909).* The results are considerably higher than
the above, viz. 0.1385 gm. Pb per 1000 cc. H2O at 20°; with increase of H2SO4
the solubility decreases rapidly.
100 cc. anhydrous hydrazine dissolve i gm. lead oxide (red) at room temp.
(Welsh and Broderson, 1915.)
Freezing-point lowering data for mixtures of PbO + PbSO4 are given by
Schenck and Rassbach, 1908. Data for mixtures of PbO + SiO2 are given by
Weiller, 1911, and by Cooper, Shaw and Loomis, 1909.
LEAD PerOXIDE PbO2.
The two forms of lead superoxide, (a) amorphous and (&) crystalline, differ
in their solubilities in sulphuric acid. One liter of very concentrated H2SO
dissolves about o.oio mol. PbO2 (&) at 22°. One liter of cone. H2SO4 contain-
ing 1720 gms. per liter, dissolves 0.0995 mol- PbO2 (a) at 22°. The solid phase
is slowly converted to Pb(SO4)2. One liter of H2SO4 containing 1097 gms. HjSO*
per liter dissolves 0.004 mol. PbO2 at 22°. The solid phase is converted more
quickly to Pb(SO4)2. In more dilute H2SO4 solutions no solubility can be de-
tected. (Dolezalek and Finckli, 1906.)
LEAD PALMITATE, LEAD STEARATE. See also p. 360.
100 cc. absolute ether dissolve 0.0138 gm. palmitate and 0.0148 gm. stearate. '
(Lidoff, 1893.)
LEAD TetraPHENYL Pb(C6H6)4.
Freezing-point data for Pb(C6H6)4 + Si(C6H6)4 are given by Pascal (1912).
LEAD PHOSPHATE (Ortho) Pbs(PO4)2.
One liter water dissolves 0.000135 gm. lead phosphate at 20° by conductivity
method. (Bottger, 1903.)
One liter of 4.97 per cent aqueous acetic acid solution dissolves 1.27 gms.
Pba(PO4),. (Bertrand, 1868.)
363 LEAD SUCCINATE
LEAD SUCCINATE PbC4H4O4.
SOLUBILITY IN WATER AND IN ALCOHOL.
(Partheil and Hiibner, 1903.)
ioo gms. H2O dissolve 0.0253 gm. PbC4H4O4 at 18°, and 0.0285 gm. at 25°.
100 gms. 95% alcohol dissolve 0.00275 gm« PbC4H4O4 at 18°, and 0.003 Sm»
at 25°.
Density of alcohol used = 0.8092.
SOLUBILITY OF LEAD SUCCINATE IN WATER.
(Cantoni and Diotalevi, 1905.)
t°. 10°. 21°. 32°. 39°. 50°.
Gms. PbC4H404 per ioo cc.
sat. sol. 0.015 0.019 0.024 0.027 0.029
LEAD SULFATE PbSO4.
SOLUBILITY IN WATER.
(Average curve from gravimetric results of Dibbits (1874), Beck and Steg-
miiller (1910) and Pleissner (1907) and conductivity results of Bottger (1903)
and Kohlrausch (1904-05).
t°. Gms. PbSO4 per Liter. t°. Gms. PbSO4 per Liter.
o 0.028 20 0.041
5 °-°3i 25 0.045
10 0.035 3° °-049
15 0.038 35 0.052
18 0.040 40 0.056 .
Results considerably higher than the above are reported by Sehnal (1909).
This author finds 0.082 gm. PbSO4 per liter at 18° and claims that the presence
of H2SO4 in the PbSO4 reduces the solubility very greatly. His results for the
solubility in presence of small amounts of H2SO4 are:
Gms. H2SO4 per 1000 cc. solu-
tion o 0.0098 0.0196 0.0980 0.4900 0.9800
Gms. dissolved PbSO4 per 1000
cc. solution at 20° 0.082 0.051 0.025 0.013 0.006 o
Sehnal also gives results showing that the solubility in water and dilute HjSO*
solutions is exactly the same at 100° as at 20°.
Data for the solubility of PbSO4 precipitates are given by deKoninck, 1907.
SOLUBILITY OF LEAD SULFATE IN AQUEOUS SOLUTIONS OF AMMONIUM ACETATE
AND OF SODIUM ACETATE.
(Noyes and Whitcomb, 1905; Dunnington and Long, 1899; Dibbits, 1874.)
In Ammonium Acetate. In Sodium Acetate.
At 25° (Nand W.). ' At 100° (D. and L.). (D.).
Millimoh per Liter. Gms. per Liter. G. NHiCaHad G. PbSO4 Gms. per ioo Cms. H2O.
NH.C.H.Q,. PbSO»." ' NHAHA. PbS04: *§£££ ShltS*' NaC2H,O2.' PbSO4. '
o 0.134 o 0.041 28 7.12 2.05 0.054
103.5 2.10 7.98 0.636 32 9.88 8.2 0.853
207.1 4.55 15.96 1.33 37 10.58 41 11.23
414.1 10.10 31.92 3.02 45 ii. 10
SOLUBILITY OF LEAD SULFATE IN AQUEOUS SOLUTIONS OF AMMONIUM
ACETATE AT 25°.
(Harden, 1916.)
Gms. per 1000 Gms. Sat. Sol. Gms. per rooo Gms. Sat. Sol.
NH«CiH,0*. PbS04. NH4C,H,0,. PbSO4. "
7.96 0.636 53.4 5.60 1. 012
15.91 i-37° 106.8 16.8 1.024
31.70 3.04 213.7 3S-9 1-045.
Milligrams Pb per 100 cc. Solution.
Normal-
Mgm. Pb
Normal-
Mgm. Pb
At 18°.
At 25°.
At 37°.
HNO3.
So?.
N»CL
per 100 cc.
Sol.
I 2.6O
3
3.80
O.I
10.48
O.I
11.19
19
22.18
28.04
O.2
17.48
0.2
18.73
35-70
42.88
54-50
0-3
23.4I
o-3
26.51
55-37
65-15
84.04
0.4
29.84
0.4
33-76
75-27
88.80
I I I . 9O
LEAD SULFATE 364
SOLUBILITY OF LEAD SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM ACETATE
AND OF SODIUM ACETATE AT 25°. (Fox, 1909.)
In Aq. Potassium Acetate. In Aq. Sodium Acetate.
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol. c ...
, * x Solid Phase. , *- ^ |°hd
CH3COOK. (CH3COO),Pb. CH,COONa. (CH3COO)2Pb. Na^SO,. Phase'
4.33 2.54 PbSO.+PbKjCSO^j 6.69 0.78 0.34 PbSO,
9-°3 3-55 6.95 0.81 0.35
17.81 5.43 11.76 2.73 1.26
26.58 9.83 16.90 5.70 2.49
28.82 11.40 19.92 8.24 3.60
28.93 19-41 21.51 10.75 4-68
In the case of the CH3COOK solutions, the double salt PbK2(SO4)2 is formed
and no SO4 ions enter the solution.
SOLUBILITY OF LEAD SULFATE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC AND
OF NITRIC ACIDS AND OF SODIUM CHLORIDE.
.(Beck and Stegmiiller, 1910.)
T_ A ur1! In Aq. HNOa In
In Aqueous HL1. ^ Tft0
Normality
of HCl.
o( = pureH20)
O.I
0.2
0-3
0.4
SOLUBILITY OF LEAD SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC ACID
AT 1 8°. (Pleissner, 1907.)
( See also Sehnal, preceding page.)
Gms. per Liter. Millimols^ per Liter. Gms. per Liter. Millimols per Liter.
HtSO4. PbSO4. " 'H2SO4. PbSO4". ' H2SO4. PbSO4. ' H2SO4. PbSO4.'
o 0.0382 o 0.126 0.0245 0.0194 0.25 0.064
0.0049 0.0333 °-°5 o.no 0.0490 0.0130 0.50 0.043
0.0098 0.0306 o.io o.ioi 0.4904 0.0052 5 0.017
SOLUBILITY OF LEAD SULFATE IN CONCENTRATED AQUEOUS SOLUTIONS OF ACIDS.
(Schultz, 1861; Rodwell, 1862.)
In Aq. H2SO4. In Aq. HCl. In Aq. HNO3.
(a) (b) (c) (a) (b) (c) (a) (b) (c)
1.540 63.4 0.003 I-°5 IO-6 0.14 i. 08 ii. 6 0.33
1-793 85.7 o.on i. 08 16.3 0.35 1. 12 17.5 0.59
1.841 97 0.039 i-n 22 0.95 1.25 34 0.78
1.14 27.5 2. ii 1.42 60 i. 01
1.16 31.6 2.86
(a) Sp. Gr. of Aq. Acid, (b) Gms. Acid per 100 Gms. Solution, (c) Gms. PbSO4 per 100 Gms. Solvent.
SOLUBILITY OF LEAD SULFATE IN CONC. SOLUTIONS OF SULFURIC ACID.
(Donk, 1916.)
Gm«. per 100 Gms. Gms. per 100 Gms.' ,
t«. Sat. Sol. Solid Phase. t°. Sat. Sol. Solid
H2S04. PbS04: "H2S04. PbS04.
O 51.2 O PbS04 IOO 6l.2 O PbSO4
O 89.4 O " +H5SO4.HeO IOO 72.5 O.I
o 97 o H2so4 loo 96.3 0.2
O 97.2 0.3 " +PbSO4 IOO 99.1 0.9
50 -50.4 o PbSO4 200 79 o "
50 '86.7 o.i 200 88.8 o.i
50 95-i 0.2 200 95.5 0.3
50 99.3 0.6 200 98.9 i.i
Additional data for highly concentrated solutions of H2SO4 are given by Ditz
and Kanhauser (1916).
365
LEAD SULFATE
SOLUBILITY OF BASIC LEAD SULFATES IN WATER AT 18°.
(Pleissner, 1907.)
Compound.
\ Basic Lead Sulfate
f Basic Lead Sulfate
LEAD PerSULFATE
Formula.
One Liter Sat. Solution Contains:
Mg. Lead Salt = Mg. Pb = Millimols Pb.
PbSO4.PbO 13.4 10.6
PbSO4.3PbO.H2O 26.2 22
Pb(S04)2.
SOLUBILITY IN AQUEOUS SULFURIC ACID AT 22°.
0.050
0.106
(Dolezalek and Finckli, 1906.)
Gms. per Liter.
"H2S04.
948
Pb(SO4)2.
0
1014
1081
1098
0.719
1.198
1-557
1130
1180
2.115
5-749
1217
9-303
Solid Phase.
PbOS04.H,0
Gms. per Liter.
H2S04.
Pb(S04)2.
1253
14.85
1352
16.17
1470
9-30
1532
9.46
1631
19.80
l698
33-34
1703
35-22
Solid Phase.
PbOSO4.H2O
Pb(S04),
The solid phase at concentrations of acid up to 1352 gms. per liter is the white
basic salt of the composition PbOSO4.H2O. In the concentration limits of
about 1470-1703 gms. H2SO4 per liter the original yellow color of the solid phase
remains unchanged.
Freezing-point data (solubility, see footnote, p. i) for mixtures of PbSO4-HLi2SO4,
PbSO4 + K2SO4 and PbSO4 + Na2SO4 are given by Calcagni and Mariotta (1912).
Results for mixtures of PbSO4 + K2SO4 are also given by Grahmann, 1913.
LEAD (Hypo) SULFATE.
SOLUBILITY OF MIXTURES OF LEAD HYPOSULPHATE AND STRONTIUM
HYPOSULPHATE AT 25°.
(Fock — Z. Kryst. Min. 28. 389, '97.)
Mol. per cent in Solution.
Grams per Liter. Rn nr nf
Mol. per cent in Solid Phase.
PbSjO,
SrSzCV
PbS2O6.
SrS2Oe. Solutions.
PbS208
SrS20(j
4H20.
•4H20.
.4H20.
.4H20.
0.0
100. 0
o.o
145.6
.1126
0-0
IOO-O
1.05
98-95
2-97
I5I.2
.1184
0.30
99-7
I5-3I
84.69
40.82
152.5
•1503
3-87
96.13
46.80
53-20
149-2
II4-5
.2147
9.84
90.16
62.30
37-70
256.1
85.0
.2889
19.26
80.74
75-75
24.25
3Io-3
67.0
•3252
23-73
76.27
78.09
21 .91
373-7
70-8
.3726
32.24
67.76
88.29
11.71
509-5
45-6
.4671
49-97
50-13
100. 0
o.oo
374-3
o.o
.6817
0-00
0-00
LEAD SULFIDE PbS.
One liter H2O dissolves 3.6.10"* gm. Mols. = 0.00086 gm. PbS at 18°, (Weigel, 1907.)
Determined by conductivity method. See also Bruner and Zawadzki (1909).
Fusion diagrams for PbS + ZnS and PbS + Ag2S are given by Friedrich
(1908). Results for PbS + Sb2S3 are given by Wagemmann (1912).
LEAD SULFONATES.
SOLUBILITY IN WATER.
Name. Formuta. *•.%£!£&.
Lead 2.5 Diiodobenzenesulfonate C^HgOs^S-sPb^HzO 20 0.77 (Boyle, 1909.)
Lead ft Naphthalene Sulfonate (C10H7SO3)2Pb.H2O 25 0.4 (Witte, '15; Euwes, '09.)
" « (doHvSOjJjPb.aHaO 24.9 4 . 195 (Euwes, 1909.)
Lead 2 PhenanthreneMonosulfonate iH,O 20 0.014 (Sandquist, 1912.)
5 3H2O 20 0.08
" 10 4H,0 20 0.14
LEAD TARTRATE
366
LEAD TAETRATE PbC4O6H4.
SOLUBILITY IN WATER.
(Caatoni and Zachoder — Bull. soc. chim. [3] 33, 751, '05; Partheil and HQbner — Arckiv. Pharm. 241.
'
A o Gms. PW^OeJ^ per . 0
ioo cc. Solution.
l8 O.OIO (P.andH.) 50
25 0.0108 " 55
35 0.00105 60
40 0.0015 65
'03.)
Gms. PbC4O(jH4 per
ioo cc. Solution.
O.OO225
O.OO295
0.00305
0.00315
Cms
IOO CC
70
75
80
85
PbC406H4 per
cc. Solution.
0.0032
0.0033
0.0038
0.0054
NOTE. — The positions of the decimal points here shown are just
as given in the original communications.
ioo gms. alcohol of 0.8092 Sp. Gr. (about 95%) dissolve 0.0028 gm
PbC4O6H4at 18°, and 0.00315 gm. at 25°. (P ^ H)
LECITHIN
ioo gms. of sat. solution in aqueous 5% bile salts contain 4.5 gms. lecithin at
I5°-2O° and 7 gms. at 37°. Lecithin is practically insoluble in water.
(Moore, Wilson And Hutchinson, 1909.)
LEUCINE CH3(CH2)3CH(NH2)COOH.
ioo cc. H2O dissolve 2.2 gms. leucine at 18°.
ioo cc. alcohol dissolve 0.06 gm. leucine at 17°.
Data for the solubility of leucine in aqueous solutions of salts at 20° are given
by Wiirgler , 1914, and Pfeiffer and Wiirgler, 1916:
LIGNOCERIC ACID.
Data for the freezing-points (solubility, see footnote, p. i) of mixtures of
lignoceric acid and other compounds are given by Meyer, Brod and Soyka, 1913.
LIGROIN.
ioo cc. H2O dissolve 0.341 cc. ligroin at 22°, Vol. of solution = 100.34, Sp. Gr.
0.9969.
ioo cc. ligroin dissolve 0.335 cc. H2O at 22°, Vol. of solution = 100.60, Sp. Gr.
0.6640. (Herz, 1898.)
LITHIUM Li.
One gm. atom Li dissolves in 3.93 gm. mols. NHS at —80°, at —50°. at —25°,
and at O°. (Ruff and Geisel, 1906.)
LITHIUM ACETATE CH3COOLi.2H2O.
Freezing-point data for mixtures of lithium acetate and acetic acid are given
by Vasilev, 1909.
LITHIUM SulfoANTIMONATE Li3SbS4.ioH2O.
SOLUBILITY IN WATER AND IN AQUEOUS ALCOHOL.
In Water. (Donk, 1908.)
Gms. Li,SbS4
t°. per^ioo^Gma. Solid Phase. t°.
In Aqueous Alcohol at 10° and 30°.
Gms. per ioo Gms.
Sat^Sol. Solid Phase. Authority.
i
i
— i
7
2
•j
12
SOL
I Ice
8 "
IO
IO
CjHjOH.
10.7
26.2
Li,SbS4.
41 . 8 Li,SbS4.icHiO (Donk, 1908.)
36.5
;
— c
I
17
5
"
10
66.2
20
.6
— IO
8
23
2
"
30
13-3
46
. 3 Li,SbS4.8iHtO
— *5
9
28
5
"
30
51-9
30
.7 "
-26
2
35
•2
"
30
54-8
29
•9
(Schreine-
—42
40
4
Ice+Li,SbS4.ioHzO
30
58.4
30
.8 "
makers and
0
45
5
LisSbS4.ioH,O
30
58.6
32
.3 " +Li,SbS«
Jacobs,
+ 10
46
9
•«
30
65.26
29
.31 Li,SbS4
1910.)
30
So
i
u
30
74-3
24
. I
SO
5i
3
M
30
79-5
20
• 5
LITHIUM BENZOATE
LITHIUM BENZOATE C6H6COOLi.
SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1910.)
Gms. Q,H5COOLi
per zoo Gms.
Sat. Sol.
27.64
28.60
28.50
27.80
26.20
23.60
100 gms. H20 dissolve about 40 gms
100 gms.. alcohol dissolve about 10 gms. CeHsCOOLi at the b. pt.
LITHIUM BORATE LizQBA.
SOLUBILITY IN WATER.
t° o 10 20 30 40 45
Gms. Li2OB20s per 100 Gms. HjO 0.7 1.4 2.6 4.9 11.12 20
(Le Chatelier, 1897.)
EQUILIBRIUM IN THE SYSTEM LITHIUM OXIDE, BORIC OXIDE, WATER AT 30°.
.' (Dukelski, 1907.)
nor fnn rime Qa+ ^rtl
Solid Phase.
Per cent
CjHsOH in s
Solvent.
JMof
at. Sol.
0
IO
.103
.088
20
.072
30
.052
40
.030
50
.003
Per cent
QHjOH in
Solvent.
da of
Sat. Sol.
Gms. C«H6COOLi
per zoo Gms.
Sat. Sol.
60
0.970
19-80
70
0.932
15.40
80
O.SOO
IO.7O
QO
0.847
6.40
95
0.823
4-50
100
0.799
2.6o
I5COOLi at
the b. pt.
(U.S. P.)
Li20.
B203.
OULLU jruoac.
7.01
LiOH.H20
7-51
2.98
"
7.71
3.38
" +Li2O.B2O3.i6H2O
7.68
3.56
Li2O.B2O3.i6H2O
5-40
2.78
"
3-47
2.42
"
2.94
2-51
"
1.58
3-27
<«
2.17
6.90
«
3-66
14.78
«
5-25
22
«
5-63
23-8
"
K.8l
6. 20
Li2O.2B203.*H2O
Gms. per 100 Gms. Sat. Sol.
1.32
0.86
B203.
3.36
2.47
0.53
2.47
2.17
2.61
5.08
13.12
16.39
30.81
4.10
27.07
3-22
15.40
i-55
15.40
1.30
0.96
0.63
14.14
11.47
4.85
o
3-54
Li20.5B20,.ioH20
B(OH),
Freezing-point data (solubility, see footnote, p. i) for mixtures of LiBOj
+ NaBO2, and LiBO2 + Li2SiO3 are given by van Klooster, 1910-11.
LITHIUM BROMATE LiBrO3.
100 gms. H2O dissolve 153.7 gms. LiBrO3 at 18°, or 100 gms. saturated solu-
tion contain 60.4 gms. Sp. Gr. of sol. = 1.833. (Mylius and Funk, 1897.)
LITHIUM BROMIDE LiBr.2H2O.
SOLUBILITY IN WATER.
(Kremers, 1858; Bogorodsky, 1894; Jones, 1907.)
IO
20
30
40
44
SO
60
80
IOO
159
— 0.46
Gms. LiBr per
100 Gms. H2O.
1.058
Solid Phase.
Ice(J)
-1.94
- 4.27
-10.3
4.274
8.678
17.80
m
-30.5
37-^4
"
~45
-30
50
80
" +LiBr.3l
LiBr.3H2O
— 10
122
"
o
+ 4
143
160
" (K)
" +UET.2W
1 66
177
191
205
209
214
224
245
266
LiBr.2H20 (K)
+LiBr.H20 (B)
LiBr. H2O (K)
LiBr.H20+LiBr (B)
Freezing-point data for LiBr + LiOH (Scarpa, 1915), for LiBr + AgBr.
(Sandonnini and Scarpa, 1913.)
loo gms. glycol dissolve 60 gms. LiBr at 14.7°. (de Coninck, 1905.)
LITHIUM CAMPHORATE 368
DiLITHIUM d CAMPHORATE Ci0Hi4O4Li».
SOLUBILITY IN AQUEOUS SOLUTIONS OF CAMPHORIC ACID AT i3.5°-i6°
AND VICE VERSA.
(Jungfleiscb and Landrieu, 1914-)
Gms. per 100 Gms. Sat. Sol.
, » s Solid Phase.
C6H14(COOH)2. C10HuO4Li2.
0.621 o Camphoric Acid C6Hi4(COOH)2
2.02 3.77
3.25 10.63 Monolithium Tetracamphorate
3.51 12.61
3.99 20.56 Dicamphorate CioHi5O4.Li.CioHi604
3-43 24.69 " ,
2.87 37 .16 Camphorate CioHi5O4Li
o 40 . 80 Dilithium Camphorate
The mixtures were kept in a cellar at nearly constant temperature and shaken
from time to time until equilibrium was reached. Additional results at i7°-23°
are also given.
LITHIUM CARBONATE Li2CO3.
SOLUBILITY IN WATER.
(Bevade, 1885; Fluckiger, 1887; Draper, 1887.)
An average curve was constructed from the available results and the following
table read from it.
Gms. LigCOa per 100 Gms. Gms. Li2C(\per 100 Gms.
*0-
Water.
Solution.
1; *
Water.
Solution.
0
i-54
1.52
40
I.I7
1.16
10
i-43
I.4I
50
1. 08
1.07
20
i-33
I-3I
60
1. 01
1. 00
25
i .29
1.28
80
0.85
0.84
30
1.25
1.24
IOO
0.72
0.71
Density of saturated solution at o° = 1.017; at J5° =
SOLUBILITY OF LITHIUM CARBONATE IN AQUEOUS SOLUTIONS OP
ALKALI SALTS AT 25°.
(Geffcken — Z. anorg. Chem. 43, 197, '05.)
The original results were calculated to gram quantities and plotted
on cross-section paper. The figures in the following table were read
from the curves.
Gms Salt Grams Li2CO3 per Liter in Aqueous Solutions of:
per Liter.
KC1O3.
KN08.
KC1.
NaCl.
K2S04.
Na2SO4.
NH4C1.
(NH4)2S04.
O
12.63
12 .63
12.63
12.63
12 .63
12.63
12.63
12.63
IO
12.95
I3-°5
13 .IO
13-4
13.9
14.0
16.0
2O-7
20
13.10
13-3
J3-5
13 .9
14.7
15.0
19.2
25.0
30
13.25
13.6
13-8
14-3
IS-4
16.0
21.5
28.2
40
13.40
13-8
14.0
14.6
16.0
16.6
23-3
30.8
<5o
13.8
14.2
14-5
16.9
17.8
26.0
35-2
80
13-6
14.0
14.4
17.7
18.6
27 .6
38.5
IOO
J3-5
13.9
14.2
18.2
19.4
28.4
41.0
120
*3-3
13-7
14.0
19.9
28.7
42.6
140
13.0
J3-3
. . .
. . .
20.4
28.8
43-5
I7O
12 .6
28.0
/
200
12.2
y
20-0
...
loo gms. aq. alcohol of 0.941 Sp. Gr. dissolve 0.056 gm. Li2CO3 at 15.5°.
One liter sat. sol. in water contains 0.1722 gm. mols. = 12.73 gms- Li2CO3 at 25°.
(Ageno and Valla, 1911.)
369
LITHIUM CARBONATE
SOLUBILITY OF LITHIUM CARBONATE IN AQUEOUS SOLUTIONS OF ORGANIC COM-
POUNDS AT 25°.
(Rothmund, 1908, 1910; see also Traube, 1909.)
The solubility in H2O = 0.1687 mols. Li2CO3 per liter = 12.47 gms. at 25°.
Gm. Mols. LijCOs per Liter in Aq. Solution of:
Aqueous Solution of:
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Amyl Alcohol (tertiary)
Acetone
Ether
Formaldehyde
Glycol
Glycerol
Mannite
Grape Sugar
Cane Sugar
Urea
Thiourea
Dimethylpyrone
Ammonia
Diethylamine
Pyridine
Urethan
Acetamide
Acetonitrile
Mercuricyanide
Freezing-point data for mixtures of Li2CO3 '+ Li2SO.4 (Amadori, 1912.)
Li2CO3 + K2CO3. (Le ChateUer, 1894.)
0.125
0.25
0.5
i
Normality.
Normality.
Normality.
Normality.
. . .
0.1604
0.1529
0.1394
O.l6l4
0-1555
O.I4I7
0.1203
0.1604
0.1524
0.1380
0.1097
0.1564
0.1442
0.1224
o . 0899
0.1600
O.I5I5
0.1366
o . i 104
0.1580
0.1476
0.1300
. . .
0.1668
0.1653
0.1606
O.I53I
0.1660
0.1629
0.1565
0.1472
0.1670
0.1647
0.1613
0.1532
0.1705
0.1737
0.1778
0.1702
0.1728
0.1752
0.1778
0.1693
0.1689
0.1661
0.1557
0.1686
0.1673
0.1643
0.1605
0.1667
0.1643
0.1600
0.1523
0.1562
o . 1460
0.1280
0.0992
0.1653
0.1630
0.1577
o . 1466
0.1589
O.I48l
0.1283
0.0937
0.1592
0.1503
0.1347
0.1091
0.1604
0.1525
0.1377
0.1113
. . .
O.l6l4
0.1520
0.1358
0.1618
0.1556
0.1429
0.1178
0.1697
0.1704
LITHIUM (Bi) CARBONATE LiHCO,.
100 gms. H2O dissolve 5.501 gms. LiHCO3 at 13°.
(Bevade, 1884.)
LITHIUM CHLORATE LiClO3.
loo gms. H2O dissolve 213.5 gms. LiClO3 at 18°, or 100 gms. sat. solution con-
tain 75.8 gms. Sp. Gr. of sol. = 1.815. (Mylius and Funk, 1897.)
ioo gms. H2O dissolve 483^13. LiClO3 at 1 5°, di6 of sat. sol. = i .82. (Carlson, 1910.)
LITHIUM CHLORAURATE LiAuCU.
10
20
30
Gms. LiAuCl4 per
ioo Gms. Solution.
57-7
62.5
SOLUBILITY IN WATER.
(Rosenbladt, 1886.)
to Gms. LiAuCU per
ioo Gms. Solution.
40
50
67.3
72
60
70
80
Gms. LiAuCli per
ioo Gms. Solution.
76.4
81
85-7
LITHIUM CHLORIDE
370
LITHIUM CHLORIDE LiCl.
SOLUBILITY IN WATER.
Cms. LiCl per 100 Gms.
(Average curve from results of Gerlach, 1869.)
Gms. LiCl per 100 Gms.
» .
Water.
Solution.
0
67
40.1
10
72
41.9
20
78-5
44
25
Bi.S
44.9
3°
84-5
45-8
I .
Water.
Solution^
40
90.5
47-5
50
97
49.2
60
103
SI.Q
80
"5
53-5
100
127.5
56
Density of saturated solution at o°, 1.255; at 15°, 1.275.
SOLUBILITY OF LITHIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID.
Results at 25°. (Here, 1911-12.)
Gms. per 100 cc. Sat. Sol.
LiCl. HC1.'
Results at o°. (Engel, 1888.)
Gms. per 100 cc. Sat. Sol.
LiCl.
HC1.
»0 IN oat. i
51
0
1.255
41-4
8.2
1.243
28.5
24.1
I.. 249
24.6
29-5
L25I
57-4
56.87
53-64
51.98
o
2.30
3-84
6.43
SOLUBILITY OF LITHIUM CHLORIDE IN AQUEOUS SOLUTIONS OF ALCOHOL AT 25°.
(Pinar de Rubies, 1913-1914.)
' The LiCl was determined by titration with AgNOs. Solutions saturated by
constant agitation for many hours. Solid phase, LiCl.r^O for all mixtures.
The anhydride, LiCl, separates only from the most highly concentrated alcohol
solutions.
Gms. per 100 Gms. Sat Sol.
Gms. per 100 Gms. Sat. Sol.
CiH6OH.
O
IO
20
30
40
LiCl.
44.9
40.9
37-25
33-3
29.4
QH5OH.
50
60
70
75
80
LiCl.
25-75
21.6
21. 1
20.8
20.75
SOLUBILITY OF LITHIUM CHLORIDE IN ETHYL ALCOHOL AT DIFFERENT
TEMPERATURES. (Turner and Bissett, 1913.)
o Gms. LiCl per 100
Gms. QjH6OH.
Solid Phase.
Solid Phase.
O
5
10
i5
17
Solvent.
14.42 LiC1.4C2H5OH
15-04
16.77
18.79
20.31
SOLUBILITY OF LITHIUM CHLORIDE IN SEVERAL SOLVENTS.
Gms. LiCl
20
24.28
LiCl
30
25.10
«
40
25-38
n
50
24.40
M
60
23.46
ft
Gms. LiCl
per 100
Gms.
Solvent.
Authority.
Solvent. t°
per 100
Gms.
Solvent.
Authority.
9-03
10-57*
4.32*
1-93*
(Turner & Bissett, 1913.)
(Andrews & Ende, 1895.)
(Patten & Mott, 1907.)
Alcohol: Alcohol:
Methyl 25 42.36 (Turner & Bissett, 1913.) Amyl 25
Ethyl 25 2 . 54* (Patten & Mott, 1904.) " ?
Propyl 25 16.22 (Turner & Bissett, 1913.) " 25
? 15.86 (Schkmp, 1894.) Butyl 25
25 3.86*(P*tten&Mott, 1904.) Glycerol 25
Allyl 25 4.38* Phenol 53
* Fused LiCl used for these determinations.
loo cc. anhydrous hydrazine dissolve 16 gms. LiCl at room temp.
(Welsh and Hroderson, 1915.)
371
LITHIUM CHLORIDE
t°.
8
28
40
60
80
IOO
SOLUBILITY OF LITHIUM CHLORIDE IN SEVERAL SOLVENTS.
(Laszczynski, 1894; deConinck, 1905.)
In Acetone. (L.)
In Pyridine. (L.) In Glycol. (de C.)
Gms. LiCl
Gms. LiCl
f.
per 100 Gms.
t°.
per 100 Gms.
(CH,)2CO.
0
4.60
46
3-76
12
4.41
53
3-12
25
4.II
58
2.14
"t°.
15
Cms. Lid
per too Gms.
C6H5N.
7-78
14-26
Cms. Lid
t°. per 100 Gms.
Sat. Sol.
15 ii
SOLUBILITY OF LITHIUM CHLORIDE IN PYRIDINE.
(Kahlenberg and Krauskopf, 1908.)
In 97% Pyridine
In Anhydrous Pyridine.
Gms. LiCl f>er 100 Gms.
Solid Phase.
LiC1.2CfiH6N
tt
u
tt
tt
' Sat. Sol. Solvent.
11.31 12.71
11.87 13.47
I I. 60 I3.IO
11.38 12.84
11.71 13.27
13.01 14.98
tr. temp, about 28°.
K- V, 3%HS°
by Volume.
.„ Gms. LiCl per TOO Gms.
Sat. Sol.
22 12.50
32 13-79
45 15-58
58 16.72
72 17.12
97 i8.35
Solvent.
14.31
15.98
18.46
2O.O8
20.66
22.48
SOLUBILITY OF LITHIUM CHLORIDE AT 25° IN MIXTURES OF:
Acetone and Benzene.
(Marden and Dover, 1917.)
Ethyl Acetate and Benzene.
(Marden and Dover, 1917.)
Gms. Acetone Gms. LiCl
per 100 Gms. per 100 Gms.
Solvent. Solvent.
Gms. Acetone Gms. LiCl
per loo Gms. per 100 Gms.
IOO
00
80
60
2.30
1.69
0.966
0.234
Solvent.
40
2O
IO
O
Solvent.
0.088
O.OI9
0.009
O
Gms. Ethyl Acetate
per 100 Gms.
Solvent.
IOO
70
Gms. LiCl
per loo Gms.
Solvent.
I.78
0.147
0.028
0.005
DISTRIBUTION OF LITHIUM CHLORIDE BETWEEN WATER AND AMYL
ALCOHOL AT 30°.
(Dhar and Datta, 1913.)
Mols. LiCl per Liter. Cl
H2O Layer c\. Alcohol Layer Cj. **
3.24 0.0347 93.37
3.06 0.0325 94.15
2.93 0.0300 97-70
2.82 O.0275 102.58
2.76 O.O250 IIO.40
Mols. LiCl per Liter. ft
H2O Layer c\. Alcohol Layer c^. **
2.68 0.0240 in. 66
2.58 0.0275 H3.40
2.34 O.020O 117
1.84 0.0125 147-2
0.65 O.003O 2l6.66
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures of lithium chloride and other compounds.
Lithium Chloride + Lithium Hydroxide (Scarpa, 1915.)
-j- Magnesium Chloride (Sandonnini, 1913, 1914.)
+ Manganese Chloride (Sandonnini and Scarpa, 1913.)
+ Potassium Chloride (Richards and Meldrum, 1917.)
" +'NaCl (Richards and Meldrum, 1917.)
+ Rubidium Chloride (Richards &Meldrum,'i7; Zemcznzny &Rambach,'lo.)
+ Silver Chloride (Sandonnini, 191 ia, 1914.)
-j- Sodium Chloride (Zemcznzny and Rambach, 1910.)
-j- Strontium Chloride (Sandonnini, 1911, 191 ia, 1914.)
-j- Thallium Chloride (Sandonnini, 1911, 1914.)
" -j- Tin Chloride (ous) (Rack, 1914.)
LITHIUM CHROMATE 372
LITHIUM CHROMATE Li2CrO4.2H2O.
LITHIUM BICHROMATE Li2Cr2O7.2H2O.
SOLUBILITY IN WATER AT 30°.
(Schreinemaker — Z. physik. Chem. 55, 79, '06; at 18°, Mylius and Funk — Ber. 30, 1718, '97.)
Composition in Weight per cent:
Of Solution. Of Residue.
%Cr03. %Li20. %Cr03. %Li2O.
o.o 7.09
6.986 7.744 4.322 18.538
16.564 8.888 10.089 19.556
25.811 10.611 15.479 21.106
33.618 12.886 24.365 19-398
37.411 14-306 44-555 i7-4ii
37.588 14.381 36.331 18.552
37-495 13-3" 5*-o75 16.384
40.280 10.858
43.404 11.809 53-793 14-070
45-I3o 9-5I5 56-085 10.190
47-945 7-951 58-029 9.238
57.031 6.432 65.560 8.733
67-73I 5-7I3 71-687 8.513
67.814 5.689 80.452 3.780
65.200 4.661
63.257 2.141 85.914 0.758
62.28
Solid
Phase.
LiOH.H2O
LiOH JI20 + Li2Cr04.2H20
Li2CrO4.2H2O
Li2CrO4.2
Li2Cr2O7.2H2O
Li2Cr207.2H20 + CrOg
CrO,
A saturated aqueous solution contains:
.49-985 Per cent Li2CrO4, or 100 grams H2O dissolve 99.94 grams
Li2CrO4 at 30° (S.).
56.6 per cent Li2Cr2O7, or 100 grams H2O dissolve 130.4 grams
Li2Cr2O7 at 30° (S.).
52.6 per cent Li2CrO4, or 100 grams H2O dissolve 110.9 grams
LiCrO4 at 18° (M. and F.).
Sp. Gr. of sat. solution at 18° = 1.574.
LITHIUM CITRATE C3H4(OH)(COOLi)3.4H2O.
100 gms. HjO dissolve 61.2 gms. Li citrate at 15°. d^ sat. sol. = 1.187.
(Greenish and Smith, 1902.)
SOLUBILITY IN AQUEOUS ALCOHOL AT 25°.
' (Seidell, 1910.)
Wt Of
Gms.
Gms.
wt. %
.CjHuoH
in Solvent.
<*25 of C3H4OH(COOLi)3.-
Sat. Sol. 4H2O per 100 Gms.
Solvent.
Wt. %
C2H6OH
in Solvent.
<Z.E of C3H4OH(COOLi)3.-
Sat. Sol. 4HjO per icx» Gms.
Solvent.
o
1.216
74-50
50
0-933
4-93
10
I.I5O
49-30
60
0.897
2.25
20
1.083
32.10
70
0.867
0.60
30
1.025
18.80
80
0.838
0.30
40
0.976
9-65
100
0.788
O.O2
373 LITHIUM FLUORIDE
LITHIUM FLUORIDE LiF.
100 gms. H2O dissolve 0.27 gm. LiF at 18°. Sp. gr. of sol. = 1.003.
(Mylius and Funk, 1897.)
F.-pt. data for LiF + LiOH and for LiOH + Lil are given by Scarpa, 1915.
LITHIUM FORMATE HCOOLi.
SOLUBILITY IN WATER.
(Groschuff, 1903.)
Gms. Mols. Gms. Mols.
to HCOOLi HCOOLi «.... p. to HCOOLi HCOOLi «,,.. p.
*• per 100 Gms. per 100 Mols. Solid Phase. t. per I00 Gms. per 100 Mols. Solld Phase>
Solution. H20. H,0. H^O.
— 20 21.14 9-28 HCOOLi.H2O 91 54.16 40.90 HCOOLi.H2O
o 24.42 ii. 18 98 57.05 45-99 HCOOLi
18 27.85 13.36 104 57-64 47-n
49-S 35-<5o 19-14 120 59.63 51.13
74 44.91 28.22
Sp. gr. sat. sol. at .18° = 1.142.
SOLUBILITY OF NEUTRAL LITHIUM FORMATE IN ANHYDROUS FORMIC ACID.
(Groschuff, 1903.)
Gms. HCOOLi
Mols. HCOOLi
t°.
per loo Gms.
Solution.
per loo Mols.
LHCOOH.
Solid Phase.
0
25-4
30
HCOOLi
18
25-9
30-9
tt
39
26.4
31-75
tt
60
26.9
32.6
"
79
27.8
34
*'
LITHIUM HIPPURATE C6H6CO.NHCH2COOLi.
100 gms. H2O dissolve about 40 gms. of the salt at 15-20°.
(Squire and Caines, 1905.)
LITHIUM HYDROXIDE LiOH.H2O.
SOLUBILITY IN WATER.
(Dittmar, 1888; Pickering, 1893.)
Gms. per 100 Gms. Gms. LiOH
t°. Solution. per 100 Gms. t°.
Gms. per too Gms. Gms. LiOH
Solution. per I00 Cms-
Li20 =
. LiOH. ' HiO.
Li20 =
LiOH.
H20.
-10.5
. .
7-
23
.
30
7-05
II
.27
12.9
— 1 8 Eutec.
ii
. 2
. .
.
40
7.29
II
.68
13
0
6
.'67
10
.64
12
• 7
50
7.56
12
.12
13-3
10
6
•74
IO
.80
12
•7
60
7.96
12
.76
13-8
20
6
.86.
10
•99^
12
.8
80
8.87
14
.21
15-3
25
6
•95
II
.14
12
•9
100
10.02
16
.05
17.5
SOLUBILITY OF LITHIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF LITHIUM
SULFOANTIMONATE AT 30° AND VlCE VERSA.
(Donk, 1908.)
Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol. Solid Phase.,, Sat. Sol. Solid Phase.
EiOIL Li3SbS4. LiOH. Li3SbS4.
II.4 O LiOH.HjO 2.1 48.3 LiOH.H20
9.1 8.3 2.1 52.1 " +Li3SbS4.ioHI0
2.3 29.9 1.4 51.8 LUSbS4.ioH,Q
O 51-3
Data for equilibrium in the system lithium hydroxide, phenol, water at 25° are
given by van Meurs, 1916.
LITHIUM IODATE
374
LITHIUM IODATE Li(IO3).£H2O.
100 gms. H2O dissolve 80.3 gms. LiIO3 at 18°, or 100 gms. solution contain
44.6 grams. Sp. gr. of sol. = 1.568. (Mylius and Funk, 1897.)
LITHIUM IODIDE LiI.3H2O.
SOLUBILITY IN WATER;
(Kremers, 1858, 1860; ice curve, Jones, 1907.)
I .
Water.
Sat. Sol.
OU11U JTUctiC.
V .
Water.
Sat. Sol.
ooiia rnase.
—0.296
1
.08
1. 06
Ice
20
165
62.
2
LiI.3H2O
— 1.218
A
.36
4.19
a
25
I67
62.
6
«
-2.70
8
•71
8.02
«
30
171
63-
i
«
- 6.14
17
.69
15-03
it
40
179
64-
2
M
-16.2
38
3i
27.70
ii
50
187
6$.
2
M
-25
48
.67
32.72
tt
60
202
66.
9
«
~59
85
!3
46
u
70
330
69.
7
M
—69 Eutec.
93
48.2
Ice+LiI.3H2O
75
263
72.
5
H
-60
IOO
50
LiI.3H20
75
m. pt.
««
—40
118
54.13
M
85
m. pt.
. . .
LiI.2H20
— 20
134
57-27
<(
80
435
81.
|
LiI.H2O
o.
151
60.2
it
IOO
481
82.
8
((
10
157
61.1
(i
1 20
590
85-
$
a
SOLUBILITY OF LITHIUM IODIDE IN SEVERAL SOLVENTS.
Solvent.
t°.
Methyl Alcohol
25
Ethyl Alcohol
25
Propyl Alcohol
25
Amyl Alcohol
25
Glycol
Furfurol
25
Nitromethane
O
n
25
* Solid phase =
LiI.4C3H7OH.
Gms. Lil per
100 Gms. Solvent.
Authority.
343-4
(Turner and Bissett,
1913.)
250.8
" "
47.52*
« «
112.5
" "
38-9
(de Coninck, 1905.)
45 -9t
(Walden, 1906.)
I.22f
«
2.52
"
f = gms. per 100 cc. sat. solution.
F.-pt. data for Lil + Agl are given by Sandonnini and Scarpa, 1913.
LITHIUM IODOMERCURATE 2LiI.HgI2.6H2O.
100 gms. sat. solution of lithium iodomercurate in water prepared by cooling a
hot solution and allowing to stand at 24.7° for 3 months, contained 1.30 gms. Li,
27.4 gms. Hg, 58 gms. I and 13.3 gms. H2O; Sp. Gr. of the sat. sol. = 3.28.
(Duboin, 1905.)
LITHIUM LAURATE, MYRISTATE, etc.
SOLUBILITY IN WATER AND IN ALCOHOL OF d = 0.797, AT 18° AND AT 25°.
(Partheil and Ferie, 1903.)
Gms. Salt per 100 cc. Sat. Solution in:
Salt.
Formula.
Water at
Alcohol at
18°.
25°-
18°.
25°.
Stearate
CnH^COOLi
O.OIO
O.OII
0.041
0.0532
Palmitate
C15H3iCOOLi
O.OII
0.018
0.0796
0.0956
Myristate
Laurate
Oleate
Ci3H27COOLi
CnH23COOLi
CnH-aCOOLi
0.0232
0.158
0.0674
0.0234
0.1726
0.1320
0.184
O.4l8
o . 9084
0.2100
0.4424-
I.OIO
375
LITHIUM LAURATE
LITHIUM LAURATE, MYRISTATE, PALMITATE and STEARATE.
SOLUBILITY OF EACH OF THESE SALTS, DETERMINED SEPARATELY, IN
SEVERAL SOLVENTS.
(Jacobson and Holmes, 1916.)
Li laurate = CnH23COOLi. Li myristate = CisH^COOLi, Li palmitate =
CH3(CH2)uCOOLi and Li stearate = CH3(CH2)16COOLi.
Excess of salt shaken with solvent for 2 hrs. in all cases. The sat. sol. was
analyzed by evaporating to dryness and weighing residue.
Gms. of Each Salt (determined separately) per
100 Gms. Solvent.
Solvent.
Abs. -Ethyl Alcohol
Methyl Alcohol
« «
a a
ti (i
Water
tt
Ether
a
•> .
Li
Li
Li
Li
Laurate.
Myristate.
Palmitate.
Stearate.
20
0.403
0.194
0.096
0.072
25-4
0.447
O.224
O.II8
0.089
35
0.546
0.278
0.142
0.106
5o
0.782
0-435
0.248
0.200
65
I.I49
0.669
0.391
0-333
15-2
3-159
1.346
0.616
0-349
25
3-773
i. 680
0.771
0-439
34-6
4-597
2.193
i. 086
0.658
50
6.088
3.281
1.652
1-057
16.3
0.154
0.027
O.OIO
0.009
25
0.187
0.036
0.015
O.OIO
35
0.207
0.042
0.015
O.OIO
50
0.280
0.062
15-8
O.OII
0.013
0.007
O.OII
25
0.006
0.004
0.007
O.OII
16
0.073
0.029
0.019
O.OII
25-7
6. in
0*046
0.032
0.028
35
0.126
0.062
0.033
0.031
49-2
0.203
0.109
0.069
0.060
15.2
0.006
0.004
0.004
0.004
14-5
0.068
0.037
0.038
0.034
25
0.064
0.034
0.024
0.029
35
0.061
0.044
0.037
0.031
50
0.061
0.045
0.036
0.044
24-5
0.026
0.013
0.015
0.012
15
0.300
0.413
0.434
0.571
25
0.376
0.447
0.508
0.706
35
0.430
0.502
0-537
0.663
Amyl Alcohol
Chloroform
Amyl Acetate
Methyl Acetate
Acetone
tt
^ The above lithium salts were prepared by adding the calculated amount of
lithium acetate to the alcoholic solutions of the respective fatty acids. The
resulting precipitates were dissolved in boiling alcohol and the solutions allowed
to stand over night in a cool place. The salts so obtained were washed and
dried.
LITHIUM TetraMOLYBDATE Li2O.MoO3.2H2O.
100 cc. sat. aqueous solution contain 43.13 gms. Li2O.MoO3.2H2O at 20°. d»
of sat. sol. = 1.44. (Wempe, 1912.)
LITHIUM NITRATE 376
LITHIUM NITRATE LiNO3.3H2O.
SOLUBILITY IN WATER. (Donnan and Burt, 1903.)
Gms. LiNO, Cms. LiNOj
t°. per 100 Cms. Solid Phase. . t°. per 100 Cms. Solid Phase.
Solution. Solution.
o.i 34.8 LiNO3.3H2O 29.87 56.42 LiNO3.3H2O
10.5 37-9 29.86 56.68
12. i 38.2 29.64 57.48
13-75 39-3 29.55 58.05
19.05 40.4 43.6 60.8 LiN03.|H2O
22.1 42.9 50.5 61.3
27-55 47-3 55 63
29-47 53.67 60 63.6
29.78 55.09 64.2 64.9 LiNO3
70.9 66.1
The eutectic Ice + LiNO3.3lI2O, is at -17.8° and about 33 gms. LiNO3 per
100 gms. sat. sol. Transition points, 29.6° and 61.1°.
Data for die system LiNO3+Li2SO4+H2O at o°, 30° and 70° are given by
Massink, 1916.
A sat. solution of lithium nitrate in acetone contains 0.343 gm. mols. = 23.67
gms. per liter at about 2O°. ^ (Roshdestwensky and Lewis, 1911.)
Freezing-point data for LiNOs + KNO3 and LiNO3 + NaNO3 are given by
Carveth, 1898. Results for LiNOa + KNO3 are also given by Harkins and Clark,
Results for LiNO3 + Li2SO4 are given by Amadori, 1913.
LITHIUM NITRITE LiNO2.H2O.
SOLUBILITY IN WATER. (Oswald, 1914.)
Gms. Gms.
r. JSSST solid Phase. t. ™°d,£r
Sat. Sol. Sat. Sol.
- 7.5 II. I Ice 38.5 55.5 LiN02.H,0
-II.7 15 42 56.9
— 21 21.2 49 60.6
— 28.8 29 49.5 6l.2 " +LiNCMH2O
— 31.3 29.4 " +LiN02.H20 65 63.8 LiN02.*H,0
-19.3 33-9 LiN02.H20 81.5 68.7
O 41-5 91 72.4
+ 19 48.90*19=1.3186.) 96 91.8
25 50-9 92.5 94-3
100 gms. H2O dissolve 10.5 gms. AgNO2 + 78.5 gms. LiNO2 at 14°. (Oswald, 1914.)
LITHIUM OXALATE Li2C2O4.
SOLUBILITY OF MIXTURES OF LITHIUM OXALATE AND OXALIC ACID IN
WATER AT 25°. (Foote and Andrew, 1905.)
Mixtures of the two substances were dissolved in water, and the solutions cooled
in a thermostat to 25°.
Gms. per 100 Gms. Solution. Mols. per 100 Mols. H20.
" HsCA. ' Li2C204. H2C204. ' Li2C2O4. ' P aS6'
10.20 ... 2.274 ... H2C2O4.2H2O
2'457 °'622 H2C204.H20 and HLiC204.H20
808 3.18 1.823 0.633
2 60 «; o* o tc6^ o 062 \
'2 ) =39-2H2C204 and
0.469 1.273 HLiC204.H20 and Li2C204
5-87 ... 1.901 Li2C2O4
100 gms. aqueous solution, simultaneously saturated with lithium oxalate and
ammonium oxalate at 25°, contain 5.75 gms. Li2C2O4 + 4.8 gms. (NH4)2C2O4.
(Foote and Andiew, 1905.)
377 LITHIUM PHOSPHATE
LITHIUM PHOSPHATE Li3PO4.
100 gms. H2O dissolve 0.04 gm. Li3PC>4. (Mayer, 1856.)
LITHIUM (Hypo) PHOSPHATE Li4P2O6.7H2O.
100 gms. H2O dissolve 0.83 gm. hypophosphate at brd. temp. (Rammelsberg, 1892.)
LITHIUM PERMANGANATE LiMn04.3H2O
100 gms. water dissolve 71.4 gms. permanganate at 16°. (Ashoff.)
LITHIUM SALICYLATE C6H4OHCOOLi.|H2O.
SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1909, 1910.)
Gms. Gms. Gms.
CzHjOHper ^B of C6H4OHCOOH.iH2O C2H5OH per
looGrns. Sat. Sol. per 100 Gms. 100 Gms.
Gms.
<Z25 of C6H4OHCOOH.iH2O
Sat. Sol. oer too Gms.
'Solvent.
Sat. Sol.
Solvent.
Sat. Sol.
0
.209
56
60
I.I04
5I-I
10
• 195
55-9
70
1.083
49-5
20
.180
55-4
80
I .056
47-5
30'
.163
54-7
90
1.026
45-8
40
.144
53-7
92.3
I .O2O
45-6
50
.124
52.5
IOO
1.027
48.2
100 gms. propyl alcohol dissolve 18.7 gms. Li salicylate (temp.?). (Schlamp, 1895.)
LITHIUM SULFATE Li2SO4.H2O.
SOLUBILITY IN WATER.
(Average curve from Kremers, 1855; Etard, 1894.)
t°.
Gms. Li2SO4 per
100 Gms. Solution.
t°.
' Gms. Li2SO4 per
zoo Gms. Solution.
t°.
Gms. Li2SO
loo Gms. So
— 20
18.4
20
25-5
50
24-5
— 10
24.2
25
25-3
60
24.2
0
26.1
30
25.1
80
23-5
10
25-9
40
24.7
IOO
23
per
ution.
SOLUBILITY OF LITHIUM-POTASSIUM SULFATE IN WATER.
(Spielrein, 1913.)
Gms. per 100 cc. Gms. per 100 cc.
t°. Sat. Sol. Solid Phase. t°. gSat. Sol. Solid Phase. -
Li2S04. K2S04. Li2S04. K2SO4.
20 35.6 3.6 Li2SO4.K2SO4+Li2SO4 60 10.6 16.3 Li2SO4.K2SO4+K2SO4
20 13.3 13.1 +K2SO4 98 30.2 9.3 " +Li2SO4
60 32.5 6 +Li2SO4 98 9 23 +K2SO4
SOLUBILITY OF LITHIUM-SODIUM SULFATES IN WATER.
(Spielrein, 1913.)
Gms. per TOO cc. Gms. per 100 cc.
^t0. ^ Sat. Sol. SoUd Phase. t8. Sat. Sol. , Solid Phase.
Li2SO4. Na2SO4. Li2SO4. NaiSO4.
O 31.4 5.9 Li2S04.Na2S04.siH20+Li2S04 33.5 25.8 13.
° 18.5 11.4 "+Na2S04 33-5 13-9 21.8
7.5 20.4 11.17 (triple pt.) 53 28 16 6 +Li2S04
16 32 9-3 -S3 16.7 27.3 ' +Na2S04
24 26 14.9 Li2SO4.Na2S04.i2H2O+Li2SO4 99 27.4 14.4
+Li2S04
+Na2S04
24 16.5 21.4 " +Na2SO4 99 14.4 25.1
32 20 16.8 (triple pt.)
There is some uncertainty as to whether all of the above results are in terms
of grams per 100 cc. or per 100 gms. of sat. solution.
SOLUBILITY OF LITHIUM SULFATE IN ABSOLUTE SULFURIC ACID.
(Bergius, 1910.)
io cc. sat. solution in abs. H2SO4 contain 2.719 gms. Li2SO4 and the crystalline
solid phase has the composition Li2SO4.7H2SO4 and melts at about 12°.
LITHIUM SULFATE 378
SOLUBILITY OF LITHIUM SULFATE IN AQ". H2S04 AT 30°. (van Dorp, 1910.)
Cms. per 100 Cms. Sat. Sol. _ ... _, Cms. per 100 Cms. Sat. Sol.
' H.£.. ' ItfCV ' S°'"mMe- ' H.SO.. ' L1.SO.. ' S°MPhaSe-
5.05 22.74 Li2SO4.H20 55 .08 13-69 LiSC>4
12.23 20.45 61.46 17.10
16.60 19.10 62.49 18.89 Li2S04.H2SO4
32.70 13.37 69.40 13.75
42.98 10.57 78-23 11.64
52.72 H.44 83.43 15.65
SOLUBILITY OF LITHIUM SULFATE IN AQUEOUS ALCOHOL AT 30°.
(Schreinemakers and van Dorp, Jr., 1906.)
Cms. per 100 Cms. Sat. Sol. Cms. per 100 Cms. Sat. Sol.
' QH.OH. ' Li,S04. ' SohdPhaSe' ' C,H5OH. ' Li,SO4. ' S°Ld P^'
o 25.1 Li2SO4.H20 47.28 3.04 Li2SO4.H2O
11.75 16.16 58.59 1.22
21.19 n-S2 69.39 0-396
29.40 8.17 80.74 o
33.31 6.66 ,94-n o
F.-pt. data for Li2SO4 + MnSO4 are given by Calcagni and Marotta, 1914:
Results for Li2SO4 + SrSO4 are given by Calcagni and Marotta, 1912. Results
for Li2SO4 + Na2SO4 and Li2SO4 + K2SO4 are given by Nacken, 1907; results for
Li2SO4 + Ag2SO4 are given by Nacken, i9O7b.
LITHIUM SILICATE Li2SiO3.
Fusion point data for Li2O + SiO2 and Li2SiO3 + ZnSiOs are given by van
Klooster, 1910-11. Results for Li2SiO3 + MgSiO3, Li2SiO3 + Na2SiO3, Li2SiO3 +
K2SiO3 and Li2SiO3 + SrSiO3 are given by Wallace, 1909.
LITHIUM TARTRATES.
SOLUBILITY IN WATER.
Cms. Salt
Salt. Formula. t°. per too Cms. Authority.
Sat. Sol.
Lithium Dihydroxytartrate Li2C4H4O8.2^H2O o 0.079 (Fenton, 1898.)
Lithium Sodium Racemic Tartrate LiNaC^Oe^H^O 20 19.97 (Schlossberg, 1900.)
" Dextro " " 20 22.55
" Potassium Racemic " LiKC^A.I^O 20 55.19
" Dextro 20 37.82
MAGNESIUM Mg. F.-pt. data for Mg+Hg. (Cambi and Speroni, 1915.)
MAGNESIUM ACETATE Mg(CH3COO)2.4H2O.
EQUILIBRIUM IN THE SYSTEM MAGNESIUM OXIDE-ACETIC ACID-WATER AT 25°.
(Iwaki, 1914.)
Cms. per too Cms. Cms. per 100 Cms.
Sat, Sol. Solid Phase. Sat, Sol. Solid Phase.
CHjCOOH. MgO. CHsCOOH. MgO.
3.36 1. 73 MgO 31.37 7.99(CH3COO)2Mg.4H20
5.65 2.93 " 36.23 8.l8 " +2.3.3
8.06 4.21 " '35-77 8-J7 2-3-3
12.46 6.54 " ,,; 40.87 7.42
15 . 46 8 . 24 " +(CH,coo)2Mg.4H2o 47 . 86 6 . 74
15.38 8.31 (CH,COO)2Mg.4H20 56.16 5.81
14.25 7.24 " 61.59 4.68
20.19 7-47 " 69.13 3.75
22.93 7 -60 " 75.93 2.85
26.61 7.74 " 82.90 , 2.23
2.3.3 = 2(CH3COO)2Mg.3CH3COOH.3H2O. More careful work in the region
of the double salt showed that a second double salt of the composition 5(CH3COO)2
Mg.ioCH3COOH.7H2O was obtained. This compound usually separated from
the more concentrated acetic acid solutions.
379 MAGNESIUM BENZOATE
MAGNESIUM BENZOATE Mg (Ce^COOJ^HjO.
100 gms. H2O dissolve 6.16 gms. Mg(C6H6COO)2 at 15° and 19.6 gms. at 100°.
(Tarugi and Checchi, 1901.)
IOO gms. H2O dissolve 3.33 gms. MgCCgHsCOO^ at I5-2O. (Squire and Caines, 1905.)
MAGNESIUM BROMATE Mg(BrO3)2.6H2O.
TOO cc. sat. solution contain 42 grams Mg(BrO3)2, or 0.15 grammols.
at 1 8°.
(Kohlrausch — Sitzb. K. Akad. Wiss. (Berlin), i, 90, '97.)
MAGNESIUM BROMIDE MgBr2.6H2O.
SOLUBILITY IN WATER.
(Menschutkin — - Chem. Centrb. 77, I. 646, '06; at 18°, Mylius and Funk — Ber. 30, 1718, '97.)
o Grams MgBr2 per 100 Gms. Grams MgBr2 per 100 Grams.
Solution. Water. Solution. Water.
— io 47.2 89.4 40 50.4 101.6
o 47-9 91-9 5° 51-0 I04-i
io 48-6 94-5 60 51.8 107.5
18 49.0 96.1 80 53.2 113.7
18 50.8 103 . 4 (M. and F.) 100 54.6 120.2
20 49-i 96-S I2° 56-° I27-5
25 49-4 97-6 140 58-° I38-1
30 49.8 99.2 160 62.0 163.1
Density of saturated solution at 18° = 1.655 (M. and F.)
Etard — Ann. chim. phys. [7] 2, 541, '94, gives solubility results
which are evidently too high.
MAGNESIUM BROMIDE ETHERATES, ALCOHOLATES, ACIDATES,
ETC.
SOLUBILITIES RESPECTIVELY IN ETHER, ALCOHOL, ACIDS, ETC., AT
VARIOUS TEMPERATURES.
(Boris N. Menschutkin. Monograph in the Russian language entitled " On Etherates and Other Molec-
ular Combinations of Magnesium Bromide and Iodide." St. Petersburg, 1907, pp. 267 and XLVIII.
Also published in the Memoirs of the St. Petersburg Polytechnic Institute, Vols. 1-7, 1904-1907, and
in condensed form in Vols. 49-62 of the Zeit. anorg. Chem., 1906-1909.)
Preparation of Material. The dietherate of magnesium bromide,
MgBr2.2(C2H5)2O (Z. anorg. Chem., 49, 34, '06) was prepared by the very gradual
addition of bromine to a cold mixture of magnesium powder and dry ether.
It is very hygroscopic and is stable only under its ethereal solution. It is decom-
posed by water and reacts with very many organic compounds as alcohols,
acids, ketones, esters, aldehydes, etc. The addition products thus formed con-
stitute the material employed in the author's succeeding studies. The mono-
etherate of magnesium bromide, MgBr2.(C2H6)2O, was prepared just as the
dietherate, but the temperature during crystallization was kept above 30°, at
which point the dietherate is converted to monoetherate. It is also precipitated
by dry ligroin.
Method of Determination of Solubility. At temperatures below 30° the
determinations were made by agitating an excess of the salt with the solvent and
analyzing the saturated solution. At the higher temperatures the synthetic
(sealed tube) method of Alexejeff (Wied. Ann., 1885) was used.
See also p. 391.
MAGNESIUM BROMIDE
ETHERATES
380
SOLUBILITY OF MAGNESIUM BROMIDE DIETHERATE, MgBr2.2(C2H6)2O, AND OF
MAGNESIUM BROMIDE ETHERATE, MgBr2(C2H3)2O, IN ETHYL ETHER, (C2H5)2O,
AT VARIOUS TEMPERATURES.
(Menschutkin. See preceding page.)
Solubility of the Dietherate
in Ether.
Solubility of the Monoetherate
in Ether.
^0 Gms. per 100 Gms. Sat. Sol.
Mols. MgBr,.
2(C2H5)2O per t<,
100 Mols.
Sat. Sol.
Gms. per 100 Gms. Sat. Sol. (£
ols. MgBr2,
2H5)20 per
:oo Mols.
Sat. Sol.
' MgBr2.2(C2H5)2O. MgBr,.
MgBr2.(C2H6)20. MgBr2. ' '
- 8
1. 08
0.6
0
.24
0
68
.8
49
.1
28.1
o
1.44
0
.8
O
•32
20
67
.2
47
•9
27.1
+ 10
2-3
i
.27
0
3°
66
•5
47
•3
26.6
14
2-95
i
.64
0
•67
40
65
•5
46
•7
26.1
16
i
•93
o
.80
60
63
.8
45
•5
25-1
18
4.14
2
•3
0
.96
80
62
.1
44
•3
24.2
20
4.86
2
•7-
I
•125
100
60
•7
43
•3
23-5
22.
.8 6.3
3
•5
I
.6
120
59
.6
42
•5
22.9
Two liquid layers separate between these con-
I4O
58
•5
41
•7
22.3
centrations of MgBr2.2(C2Hjj)2O.
158
57
•5
41
21-9
23
72.3
40
.1
36
.8
Two liquid layers separate between these con-
24
75-3
41
.8
40
•5
centrations of MgBr2.(C2H6)2O.
26
79-5
44
.1
46
.6
158
5
.8
4
.15
1.6
28
5 84.2
46
•7
54
.2
158
4
.8
3
•4
1.36
30
85.5
47
•4
56
•9
159
i
.96
i
•4
0.56
l62
0
.38
o
.27
O.II
170
0
.18
0
•13
0.05
At 22.8° and 158° the saturated solutions of the dietherate and monoetherate,
respectively, separate into two liquid layers which have at the intervening tem-
peratures the following composition. Determinations of the specific gravity of
the lower layer gave d# = 1.1628 and d%$ = 1.1492.
Gms. per 100 Gms. Solution.
t°. Lower Layer.
Upper Layer.
MgBr2.2(C2H3)2O.
MgBr2.
MgBr2.2(C2H3)2O.
MgBr2.
— 10
75-75
42
3-2
1.8
0
73-9
41
4.1
2-3
+ IO
72.2
40.1
5
2.8
20
70.8
39-3
5-9
3-3
30
69.8
38.7
6.8
3-8
40
68.8
38.2
7-7
4-3
50
68
37-8
8.5
4-7
60
67.7
37-6
9.2
5.1
70
67.7
37-6
9-7
5-4
80
68
37-8
10
5-6
90
68.6
38.1
10.2
5-7
100
69.4
38.5
10.4
5-8
120
71
39-3
10. 1
5-6
140
72.4
40.15
9.2
5.1
158
74
41
7.8
4-3
unstable
stable
38i MAGNESIUM BROMIDE
ALCOHOLATES
SOLUBILITY OF ETHYL, METHYL, PROPYL, ETC., ALCOHOLATES OF MAG-
NESIUM BROMIDE IN THE RESPECTIVE ALCOHOLS. (Menschutkin, 1907.)
These compounds were all prepared by the action of magnesium bromide
dietherate upon the several alcohols. The ether was expelled and the new alco-
holate addition product recrystallized from the respective alcohol. The solubility
determinations were made by the synthetic method.
Solubility of Solubility of Solubility of Solubility of
MgBr2.6CH3OH M
in Methyl Alcohol. in
gBr2.6C2H5OH MgBr2.6C3H7OH MgBr2.6IsoC4H9OH
Ethyl, Alcohol, in Propyl Alcohol, in IsoButyl Alcohol.
Gms. MgBr2.
t» 6CH3OH to
Gms. MgBr2.
6C2H6OH to
Gms. MgBr2. Gms. MgBr2.
6C3H7OH to 6C4H9OH
per ioo
per ioo
per ioo per ioo
Gms. Sat. Sol.
Gms. Sat. Sol.
Gms. Sat. Sol. Gms. Sat. Sol.
o 42.6 o
17.2 o
77-9 o 55-8
20 44.6 10
24.9 10
81.5 10 60.5
40 46 . 7 20
32.7 20
85.1 20 65.2
60 48 . 9 30
40-3 30
88.5 30 69.8
80 51.4 40
47.8 40
92 40 74.3
ioo 55.5 60
62.2 43
93 50 78.5
I2O 60.7 80
73-8 46
94.3 60 82.4
140 66 . 8 90
78.7 48
95-8 65 84.2
160 74 ioo
86.7 50
97.8 71 88
180 84.5 103
90 52m.pt. ioo 75 92
185 88 106
94-4
77 94-6
i90m.pt. ioo 108
.5m.pt. ioo
8om.pt. ioo
Solubility of
MgBr2.6 Iso C5HnOH
in IsoAmyl Alcohol.
Solubility of
MgBr2.4(CH3)2CHOH
in Dimethyl Carbinol.
Solubility of
MgBr2.4(CH8)3COH
in Trimethyl Carbinol.
Gms. MgBr2.
t» 6C5HUOH per
Gms. MgBr2.
to 4(CH3)2CHOH
Gms. MgBr2.
to 4(CH3)3COH
ioo Gms.
per ioo Gms.
per ioo Gms.
Sat. Sol.
Sat. Sol.
Sat. Sol.
i o 70.2
o 40
24.7m. pt. of (CH3)3COH
10 75-6
2O 42 . 2
24.4Eutec. 0.06
20 80.2
40 45
25 I
30 84.5
60 48.5
35 9-5
35 86.7
80 53-3
45 19-1
38 88.7
ioo 59
55 32.2
40 90
120 67.3
60 40.5
42 92
130 74
70 62.5
44 94-2
136 83.6
75 77
46 m. pt. ioo
138 90
79 91-5
139 m. pt. ioo
80 m. pt. ioo
MAGNESIUM BROMIDE ANILINATES.
SOLUBILITY OF MAGNESIUM BROMIDE ANILINATES IN ANILINE AT
DIFFERENT TEMPERATURES. (Menschutkin, 1907.)
The compounds were formed by the action of aniline on magnesium bromide
dietherate. The three compounds were: MgB^CeHsNH-j, MgBr2.4C6H4NH2
and MgBr2.2C6H5NH2.
Gms. MgBr2.
to 4C6HSNH2
per ioo Gms.
Sat. Sol.
IO
3-2
50
5-i
70
7-5
QO
12.8
IOO
18.5
103.5
27-5
103 tr. pt.
24
1 20
24-3
140
24-3
Solid Phase.
MgBr2.6C6H5NH2
MgBr2.4C6H5NH,
Gms. MgBr2.
4C6H8NH2
t .
per ioo Gms.
Sat. Sol.
160
26
180
28.3
200
33-5
2 2O
45
230
55
237 tr. pt.
76.3
250
77-3
260
78.1
270
79
Solid Phase.
MgBrI.4C6H4NH1
MAGNESIUM BROMIDE 382
MAGNESIUM BROMIDE PHENYLHYDRAZINATES.
SOLUBILITY OF MAGNESIUM BROMIDE. PHENYLHYDRAZINATES IN PHENYL-
HYDRAZINE.
(Menschutkin, 1907.)
(Approximate determinations.)
Gms. MgBr2.
5NHNH2
2O
40
60
80
99
Cms. MgBr2.
6QH6NHNH2
per too Gms.
Sat. Sol.
3
7
16.4
33
54-8
Solid Phase.
MgBrj.GCeHsNHNH,
IOO tr. pt.
140
180
200
Sat. Sol.
54-8
60.8
68.4
73-4
MgBr2.4QHjNH.NH2
MAGNESIUM BROMIDE COMPOUNDS with Benzaldehydeand with Acetone-
SOLUBILITY RESPECTIVELY IN BENZALDEHYDE AND IN ACETONES.
(Menschutkin, 1907.)'
The compounds were prepared by the action of benzaldehyde and of acetone on
magnesium bromide dietherate. On account of the nature of the compounds the
results are only approximately correct.
Solubility of MgBr2.3C6H5COH
in Benzaldehyde.
Solubility of MgBr2.3CH3.CO.CH3.
in Acetone.
Gms. MgBr2.
« 3QH6COH to
per ioo Gms.
Gms. MgBr2.
3C6H5COH
per ioo Gms.
Gms. MgBr2. • Gms. MgBr2.
to 3CH3.CO.CH3 to 3CH3COCH3
per ioo Gms. per ioo Gms.
Sat.
Sol.
Sat. Sol.
Sat. Sol.
Sat.:
Sol.
O
0
•7
140
I7.8
0
0.2
75
50
,
30
I
.3
145
37-5
30
0.8
76
71
.6
60
I
•9
146
65
60
i-45
80
83
•3
IOO
3
•4
148
84-5
70
2
84
89
.8
120
6
153
93-2
73
5-5
88
95
.2
130
9
•5
I5pm.pt.
IOO
74
14
92m. pt.
IOO
MAGNESIUM BROMIDE COMPOUNDS with Methylal, Ortho Ethylformate,
Formic Acid and Acetic Acid.
(Menschutkin, igo7a.)
The compounds were prepared by the action of methylal, ortho ethylformate*
and absolutely dry formic and acetic acids on magnesium dietherate. In the case
of the latter compounds the results are only approximately correct, due to their
extreme hygroscopicity.
Solubility of Solubility of Solubility of Solubility of
MgBr2.2CH,(OCH3)2 MgBr2.2CH(OC2H6)3 MgBr2.6HCOOH MgBr2.6CH3COOH
in Methylal.
in Orthoethylformate. in Formic Acid.
in Acetic
Acid.
Gms. MgBr2. Gms. MgBr2. Gms. MgBr2.
t» 2CH2(OCH3), to 2CH(OC2H6)3 to 6HCOOH
per ioo Gms. per ioo Gms. per ioo Gms.
Sat. Sol. Sat. Sol. Sat. Sol.
Gms. MgBr2.
to 6CH3COOH
' per ioo Gms.
Sat. Sol.
20
o-3
0
n. i
o
49-8
17
o-3
40
0.45
20
12.5
20
57-5
3°
i . 5
60
0.6
40
14.8
40
65-1
50
4-5
80
0-75
60
18.6
60
73-i
60
7-9
IOO
0.9
80
25-7
70
78.1
70
16.2
106
i.i
90
35
80
86
80
38.5
2 liquid layers here
95
86
95
90
57-7
106
86.2
IOO
50
88 m. pt.
IOO
IOO
71.8
108
90.8
105
66
105
80
no
95-4
no
88.5
no
89.5
112 m. pt.
IOO
114 m. pt.
IOO
112 m. pt.
IOO
383
MAGNESIUM BROMIDE
MAGNESIUM BROMIDE COMPOUNDS with Acetamide, Acetanilide and
Acetic Anhydride. (Menschutkln, 1909.)
The compounds were prepared by reaction with magnesium bromide dietherate.
Solubility of
MgBr2.6CH3CONH2
"in Acetamide.
Gms.
MgBr2.6CHr
te. CONH2 Solid Phase,
per ioo Gms.
Sat. Sol.
Solubility of Solubility of
MgBr2.6CH3CONHC6H5 MgBr2.6(CH3CO)8O
in Acetanilide. in Acetic Anhydride.
Gms. Gms.
MgBr2.6CHr MgBr2.
t°. CONHQHs Solid Phase. t°. 6(CH3COO)2O
• per ioo Gms. per ioo Gms.
Sat. Sol. Sat. Sol.
82 m.pt.ofCH3CONH2 CH3CONH2
112 m. pt. of CHsCONHQHj o
26
4
80
3
I
no
3-
7
CHsCONHQHs 2O
28
7
70
21
7 "
108
7-
7
40
31
6
60
40
"
-* n
"+MgBr2CH3- 60
35
7
ff\
CH3CONH2+MgBr2
107.
5 9
CONHQH6 80
i
50-5*
50
CH3CONH2
L20
13-
i
MgBr2.CH,CONHC6H6 ioo
48
4
70
57
8 MgBr2.CH,CONH2
140
19.
3
" 1 2O
57
8
90
60
5
160
25-
5
I30
69
8
1 10
65
180
35-
3
133
77
130
5
200
59-
5
135
85
150
80
205
73-
2
136. 5t
1 60
85
207
82.
5
"
165
90
209
ioof
"
i69f
IOO
4.
MAGNESIUM BROMIDE COMPOUNDS with Urethan and with Urea. •
(Menschutkin, 1909.)
Solubility of Magnesium Bromide Solubility of Magnesium Bromide
Urethan Compounds in Urethan. Urea Compounds in Urea.
Gms. Gms.
TMgBr2.4C2H5O- MgBr,.4CO-
t°. CONH2 Solid Phase. t°. (NH,)2 Solid Phase,
per ioo Gms. per iooj3ms.
Sat. Sol.
bat. bo
i.
49m.
pt. of urethan
C2H3OCONH2
132
m. pt. of urea COCNHj),
45
18.5
"
126
9-5
"
36-5
"
120
17.2
«
35*
43-3
" +MgBr2.6C2H3OCONH2
114
21.8
»
So
45-6
MgBr2.6CjH3OCONH2
108.
5* 24.2
CCKNH,), +MgBr2.6CO(NHj),
70
51 -3
"5
29.8
MgBrj.GCOCNHzJj
80
56-2
120
35
" t
90
66.5
127
45-5
"
75-5
130
60
"
9It
69.4
+MgBr2.4C,H,OCONH,
i3°t
58
" +MgBr2.4CO(NH2),
IOO
73-8
MgBr2.4CjH3OCONH,
145
60.7
MgBrj^COCNH,),
no
80
«
1 60
67.2
"
"5
84.1
"
165
71.4
"
120
90
"
170
83-7
M
123
IOO
"
171
96
«
* Eutec.
t tr. pt.
MAGNESIUM CAMPHORATE CioH14O4Mg.i4H2O.
SOLUBILITY OF MAGNESIUM CAMPHORATE IN d CAMPHORIC ACID AT 15°
AND VICE VERSA.
Qungfleisch and Landrieu, 1914.)
Gms. per ioo Gms. Sat. Sol
' Ci0H1404. C10H1404Mg.
3.16 10.30
3-5 16.5
3.6 16.7
1.91 15-1
o 14.25
Gms. per ioo Gms. Sat. Sol. _
C10Hlg04. ' C10H14Q^g.So
0.622 (13.5°) o CioH16O4
I . 20 I . 29
1-98 3-53
2.36 5-66
2.85 8.19
Solid Phase.
CioHlo04
" +CioH1404Mg.i4H20
CioH,404Mg.i4H20
MAGNESIUM CARBONATE 384
MAGNESIUM CARBONATE MgCO,.3H2O.
SOLUBILITY IN WATER IN PRESENCE OF CARBON DIOXIDE AT 15°.
(Treadwell and Reuter — Z. anorg. Ch. 17, 200, '98.)
cc. CO2 per too cc.
Gas Phase (at o°
and 760 mm.).
Partial
Pressure of COa
in mm. Hg.
Grams per
TOO cc. Solution.
Free CO2.
MgC03.
Mg(HC03)2.
Total Mg.
1 8. 86
143-3
O.IIQO
. . .
I.2I05
0.2016
5-47
41 .6
0.0866
I .2IO5
0.2016
4-47
33-8
0.0035
I .2105
0.2016
i-54
11.7
0.0773
I .0766
0.2016
J-3S
10.3
. . .
0.0765
0.7629
0.1492
1.07
8.2
...
0.0807
0-5952
0.1224
0.62
4-7
. . .
O.O7OI
0-3663
0.0865
0.60
4.6
0-0758
0.3417
0.0788
o-33
2-5
0-0748
0.2632
0.0655
0.21
1.6
0.0771
O.2229
0.0594
0.14
i .1
0.0710
0.2169
0.0566
0.03
o-3
0.07II
0.2036
0.0545
0.0685
0.2033
0-0536
0.0702
0-1960
0.0529
0.0625
0.2036
O.O52O
0.0616
0.1954
0.05II
...
...
0.0641
0.1954
O.O5l8
Therefore at o partial pressure of CO2 and at 15° and mean barometric pressure,
one liter of saturated aqueous solution contains 0.641 gm. of MgCO3 plus 1.954
gms. Mg(HCO3)i.
It is pointed out by Johnston (1915) that although Treadwell and Reuter made
very painstaking analyses, their mode of working did not secure equilibrium con-
ditions, a fact which is borne out by the lack of constancy of the calculated solu-
bility-product constant.
SOLUBILITY OP MAGNESIUM CARBONATE IN WATER CHARGED WITH CAR-
BON DIOXIDE AT PRESSURES GREATER THAN ONE ATMOSPHERE.
(Engel and Ville — Compt. rend. 93, 340, '81; Engel — Ann. chim. phys. [6] 13, 349, '88.)
Pressure of
C02in
Atmospheres.
G. MgCO3?
per Liter.
Pressure of
CO2in
Atmospheres o
G. MgC03* per Liter.
At
12°.
At 19°.
At
12°.
At 19°.
o-5
20.
5
.
4
• o
42
.8
I.O
26.
5
25
.8
4
•7
43-5
2.0
34-
2
33
.1(2
,i At.)
6
.0
50
.6
48.5(6
2 At.)
3-o
39-
O
37
•2(3
.2 At.)
9
.0
56.6
SOLUBILITY IN WATER SATURATED WITH CO3 AT ONE ATMOSPHERE.
(Engel.)
f. o Gms. MgCO>*
per Liter.
60 II
80 5
100 O
Dissolved as Mg(HCO3)a.
t<>.
Gms. MgCO3*
per Liter.
±y Gms.MgCO3*
per Liter.
5
36
30
21
10
31
40
17
20
26
385
MAGNESIUM CARBONATE
Data for the system magnesium carbonate-carbonic acid- water at 20°, 25°, 30°,
34° and 39° are given by Leather and Sen (1914). In connection vith these results,
it is pointed out by Johnston (1915), that it is questionable whether equilibrium
was really obtained and furthermore, the accuracy of the analytical results cannot
be trusted since the ratio of total amount of CO2 in solution, to the magnesia ia
very irregular. The results when plotted directly show great inconsistencies.
THE CALCULATED SOLUBILITY OF MgCO3.3H2O IN WATER AT 18° IN CONTACT
WITH Am CONTAINING PARTIAL PRESSURES OF CO2 FROM 0.0002 TO 0.0005
ATMOSPHERES.
(Johnston, 1915.)
It is shown that if the CO2 pressure is kept constant at P and the water evapo-
rated off so slowly at 18° that equilibrium conditions are continuously maintained,
the following amounts of Mg(OH)2 or of MgCO3.3H2O will be obtained.
Partial Pressure P
of CO2 in Atms.
O
Mols.
Cms. per Liter.
0.0087 Mg(OH)2
I3
29
45
60
97
05
12
Total Mg
p
0.00015
0.01934
O.O22I8
0.02486
0.02742
0.02868
0.02924
0.02976
SOLUBILITY OF MAGNESIUM CARBONATE IN NATURAL WATERS.
(Wells, 1915.)
(In all cases the solutions were in equilibrium with atmospheric air at 20°.)
Milligrams per Liter of Sat. Solution.
Mixture.
MgC03.3H20
0.00020
0.00025
0.00030
0.00035
0.00040
0.00045
0.00050
Mg. Free COj.
Natural Magnesite in Distilled H2O 0.018 trace 0.065
in Aq. NaCl (27.2 g. per 1.) 0.028 trace 0.086
MgCOs^BkO (equilibrium from bicarbonate end) 0.038 0.28 COc as carbonate 0.83
MgCO3.3H2O( ' under saturation ") 0.034 0.32 CO2" 0.59
SOLUBILITY OF MAGNESIUM CARBONATE IN AQUEOUS SOLUTIONS OF
POTASSIUM BICARBONATE.
(Auerbach, 1904.)
The conditions necessary for preventing changes in equilibrium due to hy-
drolysis and loss of CO2 are discussed. The mixtures were shaken from 1-4 days.
The sat. sol. analyzed for total alkali ( K -\ J by titration with standard HC1
using methyl orange as indicator. The neutralized solution was boiled to expel
CO2 and then excess o. i n NaOH added and the filtrate from magnesium precipi-
tate back titrated with o.i n HC1. The — - was calculated from the used O.I n
NaOH and the K obtained by difference.
Results at 15°.
Mols. per Liter.
Results a
Mols. per Liter.
t25°.
Solid Phase.
MgC03.3H20
«
" (labil)
" +1.1
i.i
«
Results at
Mols. per Liter.
35°.
Solid Phase.
MgCO^HjO
" (labil)
" +X.X
i.i
«<
KHC03. MgOV"0
o 0.0095 MgCOs.3HzO
0.0992 0.0131 "
0.1943 0.0167 "
0.3992 O.O2II "(labil)
0.2681 0.0192 " +1.1
0.5243 0.0097 LI
0.6792 0.0074 "
0.981 0.0028 "
i.i = MgCO3.KHCO3.4H2O.
KHCO3.
O
0.0985
O.22IO
0-3434
0.4985
0.3906
0-5893
0.6406
I.I25
MgCO3.
0.0087
0.0115
0.0149
0.0181
0.0217
0.0196
0.0128
0.0117
0.006 1
KHCO3.
O
0.1092
0.2811
0.4847
0.5807
0.5088
0.6231
0.8535
MgCO3.
0.0071
0.0098
0.0142
0.0177
0.0198
0.0184
0.0153
0.0119
Additional data for this system are given by Nanty, 1911.
Data for the solubility of MgCO3 in aq. NaCl and other salt solutions, deter-
mined by prolonged boiling and subsequent cooling of the solution out of contact
with air, are given by Gothe (1915).
MAGNESIUM CARBONATE 386
SOLUBILITY OF MAGNESIUM CARBONATE IN AQUEOUS SOLUTIONS OP
SODIUM CARBONATE AT 25°. The solutions being in equilibrium
with an atmosphere free from CO2.
(Cameron and Seidell — J. Physic. Ch. 7, 588, '03.)
Wt. of i Liter Grams per Liter. Reacting Weights per Liter.
of Solution.
Na2C03.
Mgco3:
Na2C03.
MgC03.
996.8
o.oo
0.223
o.ooo
O.OO266
1019-9
23.12
0.288
O.22O
0.00344
1047-7
50-75
0.510
0.482
o .00620
1082.5
86.42
0.879
O.82O
0.01027
1118.9
127.3
1-314
1.209
0.01570
1147.7
160.8
1.636
I .526
0.01955
1166.1
181.9
1.972
1.727
0.02357
1189.4
213.2
2.317
2.024
0.02770
SOLUBILITY OP MAGNESIUM Bi CARBONATE AND OF MAGNESIUM CAR-
BONATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AT 23°. The
solutions being in equilibrium with an atmosphere of CO2 in the
one case, and in equilibrium with air free from CO2 in the other.
(C. and S.)
In Presence of CO2 as Gas Phase. In Presence of Air Free from CO2.
Cms. NaCl
per Liter.
Gms. Mg(HCO3)2
per Liter.
Wt. of i
Liter.
Gms. NaCl
per Liter.
Gms. MgCO3
per Liter.
7-0
30.64
996.9
o.o
0.176
5^5
30.18
IOI6.8
28.0
0.418
119.7
27.88
1041 . I
59-5
0.527
163.9
24.96
1070.5
106.3
0.585
224.8
20.78
1094.5
147.4
0-544
306.6
iQ-75
1142.5
231.1
0.460
II70.I .
272.9
o-393
II99-3
331-4
0.293
SOLUBILITY OP MAGNESIUM CARBONATE IN AQUEOUS SOLUTIONS OF
SODIUM SULPHATE AT 24° AND AT 35.5°. The solutions being in
equilibrium with an atmosphere free from CO2.
(Cameron and Seidell.)
Results at 24°. Results at 35.5.°
Wt. of Gms. Na2SO4 Gms. MgCO8 Wt. of Gms. Na2SO« Gms. MgCO3
i Liter. per Liter. per Later., i Liter. per Liter. per Liter.
007-5 o.oo 0.216 995-1 0.32 0.131
I02I.2 25.12 0.586 1032.9 41.84 0.577
1047.6 54-76 0.828 1067.2 81.84 °-753
1080.9 95-68
1133.8 160.8
1157.3 191.9
1206.0 254.6
1242.0 305.1
.020 1094.8 116.56 0.904
.230 II20-4 148.56 0.962
.280 "S1-? 186.7 1-047
.338 1179.8 224.0 I. 088
.388 1236.5 299.2 1-130
MAGNESIUM CHLORATE
MAGNESIUM CHLORATE Mg(ClO3)2.6H2O.
SOLUBILITY IN WATER.
(Meusser — Ber. 35, 1416, '02.)
Mg(003)2 Mg(C103)j
per 100 Gms. per 100
Solution. Mols.H20.
Solid
Phase.
Gms. Mols.
Mg(C103)2 Mg(C10a)a
per 100 Gms. per 100
Solution . Mols . H2O .
-18
o
18
29
35
51.64
53-27
56.50
60.23
63-65
10.05
10.73
12.22
14.25
16.48
Mg(C108)2-6H30
42
65-5
39-5
61 .o
68
63.82
69.12
65-37
69.46
70.69
93 (73 -71)
16.60
20.08
17.76
21.40
22.69
(26.38)
Solid.
Phase.
Mg(C108)a.4H,0
Mg(C10a)a.3H30
Sp. Gr. of saturated sol. at + 18° = 1.564.
MAGNESIUM CHLORIDE MgCl2.
SOLUBILITY IN WATER.
(van't Hoff and Meyerhoff er, 1898; Engel; Lowenherz. Results quoted from Landolt and BCrnstein, 191 2-)
„ Gms. MgCbper too Gins SoHd
t°.
Gms. MgCljperioo Gms* Solid
t •
Solution.
Water. Phase-
Solution
. Water.
Phase.
— 10
n. i
12
•5 Ice
O
34
•5
52
.8
MgCl2.6HaO
— 2O
16.0
19
.0
IO
34
•9
53
•5
"
-30
19.4
24
.0
20
35
•3
54
•5
— 33-
6
20. 6
26
O Ice + MgCl2.i2H2O
22
35
.6
55
.2
"
— 20
26.7
36
. 5 MgCl2.i2H2O
25 36.2
56
•7
"
-16.
4
30.6
44
.04f.pt.
40
36
•5
57
•5
44
-16.
-17-
8
4
3i-6
32-3
46
47
.2
6*
*
MgCl2.i2H2O +
MgCl2.8H2O a
MgCl2.i2H20-f
MgCl2.8H2O/3
MgCl2.i2H2O +
60
80
100
37
39
42
•9
.8
.2
61
66
73
.0
.0
.0
44
44
-19
4
33-3
49
9
116
•7 46
.2
85
•5
f MgCl2.6H2O +
| MgCl2.4H2G
- 9-
- 3-
6
4
33-9
34-4
51
3*
•3
M!gC^l2.8H2O p
+ MgClo.6H2O
MgCl2.8H20 a +
MgCl2.6H2O about
152
181
6 49
5 55
.1
.8
96
126
•4
.0
MgCl2.4H2O
( MgCl2.4H2O +
\ MgCl2.2H2O
1 86
56
.1
128
.0
MgCl2.2H20
* = Unstable.
SOLUBILITY OP MAGNESIUM CHLORIDE IN AQUEOUS SOLUTIONS OP
HYDROCHLORIC ACID AT o°.
(Engel — Compt. rend. 104, 433, '87.)
Milligram Mols. p^er 10 cc. Solution.
Sp.Gr.of
Grams per Liter of Solution.
HC1.
iMgd2.
Solutions.
HC1.
MgClz.
o.o
99-55
I .362
o.o
474.2
4-095
95-5
1-354
14-93
454-8
9-5
90.0
1-344
34.63
428.6
17.0
82.5
1.300
61.97
393-o
20.5
79-o
1.297
74-74
376-2
28.5
71.0
1.281
103.9
338-3
42.0
60.125
286.4
58.75
46.25
214.2
2204.3
76.0
32-0
277.1
152.0
sat. HC1 (Ditte) 6.5
100 gms. H2O dissolve 52.65 gms. MgCl2 at 3.5°, 55.26 gms. at 25° and 58.66
gms. at 50°. (Biltz and Marcus, 1911.)
MAGNESIUM CHLORIDE
388
SOLUBILITY OF BASIC MAGNESIUM CHLORIDE IN WATER AT 25°.
(Robinson and Waggaman, 1909.)
An excess of MgO was shaken with each of 20 MgCl2 solutions at 25° for six
months and the supernatant clear solutions and solid phases with adhering liquid,
analyzed. The solutions were titrated with 0.02 n HC1 for dissolved MgO
(present as Mg(OH)2). The composition of the solid phase in each case was
ascertained by plotting the analytical results on a triangular diagram.
Solid Phase.
2MgO.HCl.SH2O
SOLUBILITY OF MIXTURES OF MAGNESIUM CHLORIDE, POTASSIUM CHLORIDE
AND OF MAGNESIUM POTASSIUM CHLORIDE (CARNALLITE) IN WATER AT
VARIOUS TEMPERATURES.
(van't Hoff and Meyerhoffer, 1899, 1912.)
Sat. Sol.
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.' gjfc^
Gms. per 100 Gms.
Sat. Sol.
MgCl*.
MgO. '
MgCl2.
MgO.
I
019
2
•36
0
00008
Indefinite
.141
17-53
0
.0024
•I
038
4
•47
o
00028
Solid Solution
.162
18.52
0
.0025
i
056
6
•79
o . 00048
.192
22.04
0
.00245
I
075
9
.02
o
00080
(C
.245
26.88
0
.0025
VI
13
• 14
0
00115
l(
.274
29.80
0
.0024
.321
34-22
o
.0030
Gms. per 100
t°. Gms. H2O.
Solid Phase.
Kind of Point on Curve.1
MeCl,.
KC1.
— II
i
. .
;
24
6
Ice +KC1
Cryohydric of KC1
- 33
6
26
" +MgCl2.i2H20
MgCl2
i2H2O
— 34
3
22
7
I
24
" +KCl+MgCl2.i2H2O
+KC1
— 21
34
9
2
03 Carnawte+MgCl2.I2H2O+KCl
Formation Temp, of
Carnallite
— O
35
5
3-02
+KC1
Point on Curve
25
38
4
4.76 + "
U ((
50
42
6
17
4- "
(( (I
(Uhlig,
1913
61
5
42
6
7
20
+ "
(( 11
*54
5
65
5
14
07
H~ "
(I «
167
5
88
i
26
-f "
M. pt. of Carnallite
25
55
5
0.83
" +MgClj.6H,O
Point on Curve
50
59
13
o
50
" + "
K It
(Uhlig,
1913-)
80
65
i
24
U _J_ «
1C it
"5
7
85
6
i
66
" + " +MgCl2.4H2O Transition Point
[Carnallite
152
5
105
7
9-93
" +MgCl2.4H20+KCl
Upper Formation Temp, of
176
126
9
16
97 MgCl2.4H2O+MgCl2.2H2O+KCl Transition Point
186
126
9
26
i
MgCl2.2H2O+KCl
Point on Curve
Carnallite = MgKCl3.6H2O.
SOLUBILITY OF MIXTURES OF MAGNESIUM CHLORIDE AND OTHER SALTS IN
Mixture.
MgCl2.6H2O+MgSO4.6H2O
MgCl2.7H2O+MgSO4.6H2O
WATER AT 25°.
(Lowenherz, 1894.)
Gms. Mols. per 1000 Mols. H2O.
104 MgCl2+i4 MgSO4
73 " +15 "
MgCl2.6H2O+MgCl2.KC1.6H2O 106 Cl2-f-i K2+io5 Mg
Gms. per Liter of Solution.
i •*"
25. Cl+4.4 SO4
19.5 Cl+5-3 S04
26.9Cl+o.3K+45.7S04
Results for all possible combinations of magnesium sulfate and potassium
chloride and of magnesium chloride and potassium sulfate are also given.
100 cc. anhydrous hydrazine dissolve 2 gms. MgCl2 at room temp. A flocculant
ppt. separates on Standing. (Welsh and Broderson, 1915.)
Freezing-point data (solubility, see footnote, p. i) for mixtures of MgCl2 and
KC1, NaCl, AgCl, ZnCl2 and SnCl2 are given by Menge (1911). Data for mixtures
of MgCl2 + SrCl2 and MgCl2 + MnCl2 are given by Sandonnini (1912, 1914).
Data for MgCl2 + MgSO4 are given by Jaenecke (1912). Data for MgCl2+TlCl
are given by Korreng (1914) and data for MgCl2+KCl and MgCl2-f HC1 are given
by Dernby (1918).
MAGNESIUM CINNAMATE
MAGNESIUM CINNAMATE (C6H6.CH.CH.COO)2Mg.H2O.
100 gms. sat. solution in water contain 0.85 gm. (C6H6CH.CHCOO)2Mg at
15° and 1.94 gms. at IOO°. (Tarugi and Checchi, 1901.)
MAGNESIUM CHROMATE MgCrO6.7H2O.
100 grams H2O dissolve 72.3 grams MgCrO< at 18°, or 100 grams solution con-
tain 42.0 grams. Sp. Gr. = 1.422. (Mylius and Funk, 1897.)
MAGNESIUM POTASSIUM OHROMATE MgCrO4.K2CrO4.2H2O.
100 grams H2O dissolve 28.2 grams at 20°, and 34.3 grams at 60°.
(Schweitzer.)
MAGNESIUM PLATINIC CYANIDE
SOLUBILITY IN WATER.
(Buxhoevden and Tamman — Z. anorg. Ch. 15, 319 '97.)
Gms.MgPt(CN)4 Gms. MgPl(CN)*
t°. per 100 Gms. Solid Phase. t°. penooGms. Solid Phase.
Solution. Solution .
— 4.12 24.90 MgPt(CN)4.6.8-8.iH2O 48.7 40-89 MfcPt(CN)4.4H2O
O
•5
26
•9
" (Red)
55
41
•33
•
5
•5
28
•65
"
58
.1
42
.15
14
18
.0
32
.46
it
69
.0
43
.40
41
36
.6-
39
•53
it
77
.8
44
,90
•
45
.0
41
•33
it
8?
•4
45
•52
M
46
.2
42
.0
•«
90
.0
45
•65
14
42
.2
40
.21
MgPt(CN)4.4H2O
93
.0
45
.04
It
46
•3
39
•85
14 (Bright Green)
96
•4
44
•33
MgPt(CN)4.2H20
100
• 0
44
.0
"
(White)
MAGNESIUM FerroCYANIDES.
SOLUBILITY IN WATER AT 17°.
(Robinson, 1909.)
One liter sat. sol. contains 1.95 gms. magnesium potassium ferrocyanide,
MgK2FeC6N6.
One liter sat. sol. contains 2.48 gms. magnesium ammonium ferrocyanide,
Mg(NH4)2FeC6N6.
MAGNESIUM FLUORIDE MgF2.
One liter of water dissolves 0.076 gm. MgF2 at 18° by conductivity method.
(Kohlrausch, 1905.)
One liter water dissolves 0.087-0.090 gm. MgF2 at 0.3° and 0.084 gm. at 27°
by conductivity method. (Kohlrausch, 1908.)
MAGNESIUM HYDROXIDE Mg(OH)2.
One liter of water dissolves 0.008 — 0.009 Sm- Mg(OH)2 at 18° by conductivity
method. (Dupre and Brutus, 1903.)
One liter of water dissolves 0.009 Sm- Mg(OH)2 at 18° by conductivity method
(Kohlrausch and Rose, 1893), 0.012 gm. (Tamm, 1910).
SOLUBILITY OF MAGNESIUM OXIDE IN AQUEOUS SOLUTIONS CONTAINING
SODIUM CHLORIDE AND SODIUM- HYDROXIDE.
(Maigret, 1905.)
Gms. MgO per Liter Solution with Added:
Gms. NaCl , * ^
per Liter. 0.8 g. NaOH 4.0 g. NaOH
125
140
160
per Liter.
0.07
0.045
none
per Liter.
0.03
none
MAGNESIUM HYDROXIDE 390
SOLUBILITY OF MAGNESIUM HYDROXIDE IN AQUEOUS SOLUTIONS OP
AMMONIUM CHLORIDE AND OF AMMONIUM NITRATE AT 29°.
(Herz and Muhs — Z. anorg. Ch. 38, 140, '04.)
NOTE. — Pure Mg(OH)2 was prepared and an excess shaken with
solutions of ammonium chloride and of ammonium nitrate of different
concentrations.
..Concentration of ^Sg^d Normality of; Grams per Liter
^Wo?™^ °'^™^r 'Mg(OH), NH.C1'. •IWOH^HH.O:
.7 (NH4C1) 0.09835 0.156 0.388 4.55 20.86
0.466 " O.IIOS 0.108 0.250 3.15 13.39
0.35 " 0-09835 0.089 O.I72 2.6o 9-21
0.233 " 0.1108 0.0638 0.106 1.86 5.67
0.175 " 0.1108 0.049 0-0771 i-43 4-i3
0.35 (NIL^NOs) O.IIoS 0.0833 O . l834(NH*NOt)2 -43 14 -69 (NIL^NOs)
0.175 " O.IIOS 0.04950-076 " 1.45 6.09
MAGNESIUM IODATE Mg(IO3)a.
SOLUBILITY IN WATER.
(Mylius and Funk — Ber. 30, 1722, '97; Wiss. Abh. p. t. Reichanstalt 3, 446, foo.)
Gms. Mols. Gms. Mols.
to Mg(I03)2 Mg(I03)2 Solid to Mg(I03)2 Mg(I03)2 Solid
per ioo per TOO Mols, Phase. per 100 per 100 Mols, Phase.
Gms. Solution. H2O. Gms. Solution. H2O.
O 3-1 0.15 MgaQs^.ioHjjO o 6.8 0.34 Mg(IOa)2.4H2O
20 10.2 0-55 10 6.4 0.30
30 17.4 i. oi 18 7.6 0.40
35 2I-9 I-35 20 7.7 0.40
50 67.5 10.0 35 8.9 0.47
63 12.6 o . 69 M
ioo 19.3 1.13
Sp. Gr. of solution sat. at 18°= 1.078.
MAGNESIUM IODIDE MgI2.8H2O.
SOLUBILITY IN WATER. (Menschutkin, 1905, 1907.)
The salt was prepared by the action of water upon magnesium iodide dietherate
(see p. 391) by which the octrahydrate and not the hexahydrate is formed. The
crystals of this hydrate melt at 43.6°. The solubility determinations were made
by the synthetic method.
Gms. per 100 Gms. Sat. Solution.
Solid Phase.
MgI2.8H2O
1 ' (Mylius and Funk, 1897.)
u
((
MgI2.6H20 =
= Mgl,.
O
76
54-7
18
59.7 W-i.909)
20
81
58.3
40
88
63.4
43.5tr.pt.
90.8
65-4
43
89.8
64.7
80
90-3
65
120
90.9
65-4
160
91.7
66
200
93-4
67.2
215
94-3
67.9
" +MgI2.6H20
MgI2.6H2O
391 MAGNESIUM IODIDE
MAGNESIUM IODIDE ETHERATES, ALCOHOLATES, ACIDATES, etc.
SOLUBILITIES RESPECT/VELY IN ETHER, ALCOHOL AND ACID SOLVENTS AT
VARIOUS TEMPERATURES.
Boris N. Menschutkin. Monograph in the Russian Language entitled "On Etherates and Other Molec-
ular Combinations of Magnesium Bromide and Iodide," St. Petersburg, 1907, pp. 267 -+- XL VIII.
Also published in "Memoirs of the St. Petersburg Polytechnic Institute," vols. 1-7, 1904-07 and in
condensed form in vols. 49-67 of the Zeit. anorg. Chem., 1906-09.
Preparation of Material. The dietherate of magnesium iodide, MgI2.2C4Hi0O,
was prepared by the very gradual addition of iodine to a mixture of magnesium
and dry ether. The reaction is not so violent as that which takes place during
the preparation of the magnesium bromide dietherate (see p.~379). Two liquid
layers are present at the end of the reaction and by slight cooling beautiful white
needle-like crystals separate from the lower one. The growth of these crystals
is also accompanied, as in the case of the magnesium bromide compound, by an
evolution of ether droplets. Magnesium iodide dietherate is very hygroscopic,
it is less stable than magnesium bromide dietherate, and becomes yellowish even
after several hours, and brown after a day, owing probably to separation of
iodine. As in the case of the magnesium bromide compound it reacts with very
many organic compounds as alcohols, acids, ketones, etc., with liberation of ether
and formation of addition products. These latter constitute the material used
for the following solubility studies.
Method of Determination of Solubility. The synthetic (sealed tube)
method of Alexejeff (Wied. Ann., 1885) was used almost exclusively.
Explanation of Results. As is seen* from the following table, the solubility
increases much more rapidly with temperature than in the case of magnesium
bromide dietherate, especially in the vicinity of the melting point of Mgl2.2C4H:oO
under its ethereal solution, which is at 23.6°. At this temperature there appears
two layers, the lower one of which may be considered as a solution of ether in
dietherate, and the upper one as a solution of the lower layer in ether. By in-
crease of temperature a point is reached, at which both layers are miscible in all
proportions (critical point). In the case of magnesium bromide dietherate no
such critical point could be obtained. Both layers may be cooled below 23.6°,
but only to about + 15° since here spontaneous crystallization of the dietherate
almost always occurs, and the temperature rises to 23.6°. The great tendency
to crystallize is probably due to the difference between the composition of the
lower layer and of the saturated solution of the dietherate. The determinations
in the vicinity of the critical point were quite difficult to make on account of the
considerable opalescence which occurred and also the formation of a white
substance, the nature of which was not ascertained. The critical concentration,
as determined by means of the law of straight averages of Cailletet and Mathias,
was approximately 40.3 per cent MgI2.2(C2H5)2O; the temperature, 38.5°. At
concentrations of MgI2.2C4HioO greater than 54 per cent, a single liquid is again
formed and the solubility curve can be followed up to the melting point of the
dietherate at 51°.
MAGNESIUM IODIDE
392
SOLUBILITY OF MAGNESIUM IODIDE DIETHERATE IN ETHER AT DIFFERENT
TEMPERATURES. (Menschutkin, 1906.)
Cms. per 100 Cms. Mols. MgI2.2(C2H6)2O
per I00 Mols.
t°. Sat, Sol. per loo Mols. Solid Phase.
5-4 2.2 1.45 0-39 MgI2.2(C2H5)2O
ii. 8
iS-6
18.1
20.4
22.2
23-6
Between these two concentrations of MgI2.2(C2H6)2O two liquid layers separate
(see below).
23-6 54.4 35-5 J7-l
25 73
^gIZ.2(CjH6)2
O = MgI2.
Sat. Sol.
2.2
I .45
0.39
3-7
2-43
0.66
5-3
0.96
8.3
5-4
1.55
n. 6
7-55
2.24
17-3
11.28
3.56
22
14.4
4.67
30
35
40
45
5i.Sm.pt.
82.5
87
89.6
93-5
IOO
47.6
54
57
58.6
61.2
65.2
42.9
53-4
60.4
71-4
100
At 23.6° the saturated solution separates into two liquid layers which have
the following composition at different temperatures.
Cms. per 100 Cms. Solution.
unstable
u
stable
«
u
it
MAGNESIUM IODIDE ALCOHOLATES and ANILINATE.
SOLUBILITY OF EACH IN THE RESPECTIVE ALCOHOLS OR ANILINE. (Menschutkin.)
4.0 Lower Layer.
MgI2.2(QH6)20 = MgI2.
Upper Layer.
Mgl^CQH-^O = Mgl,.
15
54-4
35-5
20.5
13-4
2O
54-4
35-5
21-5
I4.I
25
54-4
35-5
22.5
14.7
30
54-4
35-5
23-5
15-4
35
54-1
35-3
26
17
36
53-5
34-9
27
17.7
37
52.2
34-2
28.5
lS.1
38
So-5
33-i
32
21
38 . 5 cnt. temp.
40.3
26.3
40-3
26.3
MgI2.6CH3OH
in Methyl Alcohol
Gms.
to MgI2.6CH3OH
per loo Gms.
MgI2.6C2H5OH
in Ethyl Alcohol.
Gms.
to MgI2.6C2H5OH
per 100 Gms.
MgI2.6C6H5NH2
in Aniline.
Gms.
to MgI2.6C8H5NH2
per 100 Gms.
MgI2.6(CH3)2CHOH
in Dimethyl Carbinol.
Gms.
to MgI2.6(CHj)r
* ' CHOH oer 100
Sat. Sol.
Sat. Sol.
Sat. Sol.
Gms. Sat. Sol.
O
49.6
0
21.9
0
3-3
10
57.1
20
52.6
2O
33-2
60
3-9
30
60
40
55-3
40
44-4
IOO
5
50
63.3
60
58.8
60
55-3
130
8.5
70
67
80
60.6
80
65.5
150
17-5
90
71.2
IOO
63.3
IOO
74-7
170
38
no
76.2
1 20
66.2
120
82.7
180
S2
120
79-4
140
69.5
130
87.2
i88J
64-5
130
84.8
160
73-2
I4O
93-3
200
65.9*
136
91.7
180
77.1
143
96
210
67.2*
I38f
IOO
200
8i.S
146. st
IOO
230
69.8*
Solid Phase, Mgl^HjNH,. f M. pt. I Tr. pt. ,
393
MAGNESIUM IODIDE
MAGNESIUM IODIDE COMPOUNDS.
SOLUBILITY OF MAGNESIUM IODIDE COMPOUNDS WITH BENZALDEHYDE,
ACETONE, ACETAL, AND ACETIC ACID IN EACH OF THESE LIQUIDS.
fc(Menschutkin.)
MgI2.6C6H5COH MgI2.6CH3COCH3 MgI2.2CH3CH- MgI2.6CH3COOH
in Benzaldehyde. in Acetone. (OC2H6)2 in Acetal. in Acetic Acid.
Gms. MgI2.- Gms. MgI2.- Gms. MgI2.- Gms. Mglj.-
to 6C,H5COH to 6CH3COCH3 to 2CH3CH(OC2H6)2 fa 6CH3COOH
per loo Gms. per 100 Gms. per 100 Gms. Der 100 Gms-
Sat. Sol.
Sat. Sol.
Sat. Sol.
Sat. Sol.
0
3-2
0
4-9
20 0.15
20
0.6
20
3-8
30
6.7
60 0.45
40
2
40
5-3
50
8-3
77 0.60
60
5
60
7-7
60
10.2
(Between these two con-
70
9-5
80
n
70
15-2
centrations the mix-
80
18.5
IOO
18.5
80
28.6
ture separates into two
95
42
no
26.5
85
40
liquid layers.)
105
54-5
120
40
90
59-2
77 92
65
125
53
95
80
79 93-7
125
73-8
130
74-5
IOO
92-5
81 95-5
85
136
94.2
105
98.5
83 97-3
140
94
I39m.pt. IOO Io6.5m.pt. IOO 86m.pt. IOO I42m.pt. IOO
^On account of the properties of these molecular compounds, their great hygro-
scopicity, etc., the solubility determinations are not strictly accurate in all cases.
SOLUBILITY OF MAGNESIUM IODIDE COMPOUNDS WITH FORMIC AND ACETIC ACID
ESTERS IN THE RESPECTIVE ESTERS.
(Menschutkin.)
in Ethyl Formate, in Methyl Acetate.
in Ethyl Acetate. in Propyl Acetate.
Gms. MgI2.- Gms. MgI2.-
to 6HCOOC2H5 to 6CH3COOCH,
Gms. MgI2.- Gms. Mgl,.-
to eCHsCOOQHj to 6CH3COOC3H7
per loo Gms. ' per 100 Gms.
per too Gms. per 100 Gms.
Sat. Sol. Sat. Sol.
Sat. Sol. Sat. Sol.
o 15.1 o 0.4
o 3.2 o 4.1
10 17.4 60 0.75
20 4.8 20 5.4
20 20.5 90 0.9
40 8.6 30 6.5
30 25 loo 1.8
50 13-7 35 7-8
40 31.8 103 2.4
55 21.5 40 19
50 44 (Two layers here.)
60 38 45 46
60 68 103 74.2
65 63.5 50 72.5
7o.5m.pt. loo no 81.7
70 90.5 55 88.2
120 98
75 92-7 6° 96
I2Im.pt. IOO
78.5m.pt. IOO 65m.pt. IOO
MgI2.6CH3COO (iso) C4H9
in Isobutyl Acetate.
MgI2.6CH3COO (iso) C6HU
in Isoamyl Acetate.
Gms. MgI2.6CHr
t°. COO (iso) C4H9
per loo Gms. Sat. Sol.
Gms. MgIv6CHr
te. [COO (iso) CSHU
per loo Gms. Sat. Sol.
o 10.5
o 7.7
20 13.6
20 II.5
40 17.6
40 20 . 9
60 24 . 9
45 25.5
70 33-7
5° 33-2
80 52
55 47-8
85 < 89
57-5 63
87.5m.pt. IOO
6om.pt. IOO
MAGNESIUM IODIDE
394
MgI2.6CH3CN
in Acetonitrile.
MgI2.6CH3CONH2
in Acetamide.
Gms. MgI2.-
to 6CH.,CNper *o
Gms. MgI2.-
^CH3 CONHj Solid Phase
t° 6:
ioo Gms.
per ioo Gms.
* .1
Sat. Sol.
Sat. Sol.
0
37-2
82m
. pt. of acetamide
49 n
30
49.8
70
28 CHjCONH,
45
50
58.2
58
46.7 "
39
70
67.9
49*
56 . 5 ' +MgI2.6CHaCONH2 32*
75
71.7
80
63.4 Mglj 6CH3CONH,
40
80
76.5
130
76
60
85
83
160
85-5
80
89
170
90.8
86
i77t
IOO
87!
* Eutec.
t m. ]
SOLUBILITY OF MAGNESIUM IODIDE COMPOUNDS WITH ACETONITRILE, ACETAMIDE
AND URETHAN IN THESE LIQUIDS. (Menschutkin.)
MgI2.6NH3COOC2H6
in Urethan.
Gms. MgI2.-
™°GS?' ^id Phase.
Sat. Sol.
pt. of urethan
27.5NH3COOQH5
45
51.8 " +MgI2.NH3COOC2H5
55 MglvNHsCOOCjHj
64.7
78.8
92.5
IOO
t.
MAGNESIUM IODOMERCURATE MgI2.2HgI2.7H2O.
The sat. solution in water at 17.8° has the composition MgI2.i.29HgI2.n.o6H2O
and Sp. Gr. 2.92. (Duboin, 1906.)
MAGNESIUM DiLACTATE Mg(C6H8O6).6H2O racemic, Mg(C6H8O6).3H2O,
inactive.
SOLUBILITY OF RACEMIC AND OF INACTIVE MAGNESIUM DILACTATE IN WATER.
(Jungfleisch, 1912.)
ioo gms. H2O dissolve 7 to 8 gms. racemic and 2.28 gms. inactive lactate at 15°.
MAGNESIUM LAURATE, MYRISTATE, PALMITATE and STEARATE.
SOLUBILITY OF EACH IN SEVERAL SOLVENTS, (jacobson and Holmes, 1916.)
Gms. Each Salt Determined Separately per ioo,Gms. Solvent.
Solvent.
Water
tt
u
tt
Abs. Ethyl Alcohol
Methyl Alcohol
Ether
Ethyl Acetate
Amyl alcohol
Amyl Acetate
u
tt
tt
t°.
Mg Laurate
Mg Myristate
Mg Palmitate
Mg Stearate
(C11H23COO)Z
Mg.
• (CnHtfCOO),-
Mg.
(CH3(CH2)M-
COO)2Mg.
(CHs(CHj)r
COO)2Mg.
15
O.OIO
0.006
0.005
0.003
25
0.007
O.OO6
O.OOS
O.OO4
35
O.OIO
O.OO7
0.006
O.OO7
So
0.026
0.014
o . 009
0.008
0.519
0.158
0.034
O.OI7
25
0.591
0.236
0.058
O.O23
35
0.805
0-373
0.085
0.031
50
1.267
0-577
O.I5I
. . .
15
1.095
0.571
0.227
0.084*
25
1.108
0.763
0.36
O.IOO
S1^
0.50
0.166
25
0.015
O.OIO
O.OO4
0.003
15
0.004
0.004
0.004
0.004
35
O.OII
O.OIO
0.007
0.008
50
0.024
O.O2I
0.013
15
0.191
0.086
0.043
0.014
25
0.236
0.145
0.066
0.018
35
1.481
0.438
O.IO4
0.039
50
4.869
1.893
0.263
0.105
15
0.119
0.063
0.039
0.029
25
0.162
0.073
0.045
0.030
34-6
0.259
O.IO5
0.057
0.046
50
1-939
0.605
0.216
0.115
395
MAGNESIUM NITKATE Mg(NO3)2.
MAGNESIUM NITRATE
SOLUBILITY IN WATER.
(Funk — Wiss. Abh. p. t. Reichanstalt 3, 437, 'oo.)
t°
Gms.
Mg(N03)2
per 100 Gms.
Mols.
Mg(N03)2
per 100 Mo]
, Solid
is. Phase.
Gms.
Mg(N03)2
t . per 100 Gms.
Mois.
Mg(NOs
per loo Ik!
,)2 Solid
lols. Phase.
Solution.
H20.
Solution.
H20.
-23
35
•44
6
.6
Mg(N03)2.9H20
40
45
.87
10.
3
Mg(NOa)2^]
-20
36.19
7
.0
"
80
.69
14.
6
"
-18
38
•03
7
•4
"
90
57
.81
16.
7
"
-18
38
•03
7
•37
Mg(NO3)2.6H2O
89
63
.14
20.
9
)
~ 4
•5 39
•50
7
.92
"
77-5
65
.67
23-
2
U
0
8
.08
"
67
6?
•55
25-
I
+18
42
•33
8
•9
"
*
Reverse curve-
Sp. Gr. of solution saturated at 18° = 1.384.
The eutectic is at —29° and 34.6 gms. Mg(NO3)2 per 100 gms. sat. solution.
Fusion-point data for Mg(NOs)2 + Zn(NOs)2 are given by Vasilev (1909.)
Results for Mg(NO3)2 + HNO3 are given by Dernby (1918).
MAGNESIUM OLEATE (CH3(CH2)13CH:;CH.CH2COO)2Mg.
One liter H2O dissolves about 0.23 gm. oleate (soap). (Fahrion, 1916.)
100 gms. glycerol (d 1.114) dissolve 0.94 gm. oleate. (Asselin, 1873.)
MAGNESIUM OXALATE MgC2O4.2H2O.
One liter of water dissolves 0.3 gm. MgC2O4 at 18° (conductivity method).
(Kohlrausch, 1905.)
MAGNESIUM^ OXIDE MgO.
Fusion-point data (quenching method) for MgO + SiOg are .given by Bowen
and Anderson, 1914.
MAGNESIUM PHOSPHATE MgHPO4.3H2O.
SOLUBILITY OF MAGNESIUM PHOSPHATE IN AQUEOUS SOLUTIONS OF PHOSPHORIC
ACID AT 25°. (Cameron and Bell, 1907.)
The mixtures were constantly agitated for two months and the clear solutions
analyzed for magnesia and phosphoric acid.
^25 Of
Sat. Sol.
Gms. per Liter. c VJ
Phase. Sa^ °JL
Gms. p
er Liter.
Solid Phase.
MgO.
P206.
MgO.
P2O5.
0.207
0.486 MgHPO4.3H2O
109.5
439 MgHPO4-3H2O
0.280
0.732
1.470
122.6
498
. . .
0-553
1.917
129.9
546.5 "
1.438
4-85
140
584
.006
2.23
7-35
1-595
146.8
623.3
.017
4-73
16.84
147-3
625.9
.042
11.19
38.59
. . .
150.3
645.8
.069
17-33
61.21
. . .
155-5
680.7
V
.109
26.09
93-09
. . .
1 60
700
+MgH4(P04)2.XH20
.144
37-40
130.7
1.626
87.1
779.6
MgH4(PO4)2.XH2O
.285
75-5
281.8
1.644
77.1
809/6
"
1.654
7O.6
835.1
"
MAGNESIUM (Hypo) PHOSPHATE Mg2P2O6.i2H2O.
One liter of water dissolves 0.066 gm. hypophosphate. (Salzer, 1886.)
One liter of water dissolves 5 gms. magnesium hydrogen hypophosphate,
MgH2P2O6.4H2O. (Salzer.)
MAGNESIUM SALICYLATE Mg(C7H6O3)2.4H2O.
loo gms. sat. solution in water contain 20.4 gms. salicylate at 15° (14.3 gms.
Squire and Caines, 1905), and 79.7 gms. at 100°. (Tarugi and Checchi, 1901.)
loo gms. 90% alcohol dissolve 0.6 gm. salicylate at I5°-2O°. (Squire and Caines, 1905.)
MAGNESIUM SILICATE 396
MAGNESIUM SILICATE MgSiO,.
Fusion-point data for mixtures of MgSiOs + MnSiOs are given by Lebedew
(1911). Results for MgSiO3 + Na2SiO3 are given by Wallace (1909).
MAGNESIUM FLUOSILICATE MgSiF6.6H2O.
One liter of water dissolves 652 gms. of the salt at 17.5°.
= 1-235.
Sp. Gr. of solution
(Stolba, 1877.)
MAGNESIUM SUCCINATE C4H4O4Mg.5H2O.
100 gm£. sat. solution in water contain 24.35 gms. succinate at 15° and 66.36
gms. at I OO°. (Tarugi and Checchi, 1901.)
MAGNESIUM SULFATE MgSO4.7H2O.
SOLUBILITY IN WATER.
(Results by several investigators. 4th Ed. Landolt>nd Bornstein, " Tabellen,"
1912.)
Gms. MgSO4
Gms. MgSO4
t°. per 100 Gms. Solid Phase.
t°. per 100 Gms. Solid Phase.
Sat. Sol.
Sat. Sol.
Unstable Portions of Curve.
— 2.9 13.9 (i) ice
-8.4 23.6 (l) Ice
—3.9 19. (2) " +MgSO4.i2H2O
— 5 19 (12) " -fMgSO4.7H2O rhomb.
+ 1.8 21. 1 (2) MgSO4.i2H20+MgS04.7H2O
o 20 . 6 (3) MgSO4.7H2O rhomb.
10 23 . 6 (3) MgSO4.7H2O (rhombic)
o 25.8 (3) " 0 hexagonal
20 26 . 2 ;
0
+10 27.9 3
25 26.8 t
[
20 30 3
30 29 . %
0
o 29 3
MgS04.6H,0
40 31-3 (s)
10 29 . 7 (3
«
48 33 (<
) +MgSO4.6H,O
20 30.8 (3
50 33-S ('
7 MgS04.6H2O
30 31.2 (7
55 34-3 (
1
70 37-3 (5
60 35-5 (5)
80 39-i (S)
68 37 (8) " +MgS04.H,0
90 40.8 (5)
80 38.6 (7) MgS04.H20
100 42.5 (5)
83 40.2 (9)
99.4- 40.6(10)
164 29.3 (n)
188 20.3 (n)
. (i) de Coppet, 1872; (2) Cottrell et al, 1901; (3) Loewel, 1855; (4) Basch, 1901; (5) Mulder;
(6) Van der Heide, 1893; (7) Smith, 1912; (8) Van't Hoff, 1901; (9) Geiger, 1904; (10) Meyerhoffer,
1912; (n) Etard, 1894; (12) Guthrie, 1876. See also Tilden, 1884.
Data for densities of aq. MgSO4 solutions are given by Barnes and Scott, 1898.
SOLUBILITY OF MAGNESIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM
SULFATE AT 25° AND VICE VERSA.
(Van Klooster, 1917.)
rime r\fir Tnr* Clmc Qof Qrtl /~lr*-»p r\av Y ^/-* Clrrtv Qnf Q/-»1
Solid Phase.
MgS04.
K2S04.
•» DOI1U 1 IKISC.
MgS04.
K2S04.
26.76
0
MgS04.7H,0
13.26
10.34
26.67
1.68
"
12.88
IO.5I
26.57
2-34
"
12.68
10.70
26.36
3-76
«
12.06
10.77
26.39
4.02
" +MgK2(S04)2.6H20
10.69
10.84
18.76
7.02
MgK,(SO«),.6H|Q
7.8
II .IO
16.36
8-43
"
4
11.03
I4.27
9-63
"
o
10.77
loo gms. 95% formic acid dissolve 0.34 gm. MgSO4 at 19°.
+K2S04
K2S04
(Aschan, 1913.)
397 MAGNESIUM SULFATE
SOLUBILITY OF MAGNESIUM SULFATE IN METHYL AND ETHYL ALCOHOLS
(de Bruyn, 1892.)
Solvent. t°. Per 100 Cms. Solvent. Solvent. t°. Per 100 Gms. Solvent.
Abs. CHaOH 18 1.18 gms. MgSO4 93% Methyl Ale. 17 9.7 gms. MgSO4.7H,O
17 41 " MgS04.7H,0 50% " " 3-4 4.1 "
3-4 29 " " Abs. CijHsOH 3 1.3 "
SOLUBILITY IN AQUEOUS ETHYL ALCOHOL.
(Schiff, 1861.)
Weight per cent Alcohol 10 20 40
Gms. MgSO4.7H2O per 100 gms. solvent 64.7 27.1 1.65
SOLUBILITY OF MAGNESIUM SULFATE IN SATURATED SUGAR SOLUTION AT 31.25°.
(Kohler, 1897-)
ioo gms. saturated aqueous solution contain 46.52 gms sugar + *4 Sms.
MgS04.
ioo gms. water dissolve 119.6 gms. sugar + 36 gms. MgSO4.
Data for the system magnesium sulfate, phenol, and water are given by Tim-
mermans, 1907.
Fusion-point data for mixtures of MgSO4 + K2SO4 are given by Ginsberg,
1906; Nacken, i9O7a and Grahmann, 1913. Results for MgSO4 + NajSO4
are given by Nacken iox)7b.
MAGNESIUM POTASSIUM SULFATE MgK2(SO4)2.6H2O. ,
SOLUBILITY IN WATER.
(Tobler, 1855.)
t°- o° 20° 30° 45° 60° 75°
Gms. MgK2(SO4)2 per
icogms. H2O 14.1 25 30.4 40.5 50.2 59.8
ioo gms. H2O dissolve 30.52 gms. MgK2(SO4)2.6H2O at 15°. (Lothian, 1909.)
MAGNESIUM SULFITE MgSO3.6H2O.
10 gms. cold water dissolve 1.25 gms. sulfite; ioo gms. boiling water dissolve
0.83 gm. (Hager, 1875.)
IOO gms. H2O dissolve I gm. sulfite at 15°. (Squire and Caines, 1905.)
MAGNESIUM SULFO NATES.
SOLUBILITY IN WATER AT 20°.
(Sandquist, 1912.)
r A Gms. Anhydrous Salt
Compound. p^ JQO
Magnesium -2-Phenanthrene Monosulfonate 6H2O 0.051
-3- " " 4H2O 0.116
-10- " " 5H2O 0.22
MALAMINIC ACID
398
MALAMINIC ACID CH2(OH)COOH:jCH2CONH2, CH2COO.NH3.CHCOOH.
SOLUBILITY IN WATER AT 18°. (Lutz, 1902.)
Compound.
d |8 Malaminic Acid
M,p,.
149
U9
148
7.52
7-5°
4.02
+9 . 70
-9-33
MALEIC ACID COOHCHfCH.COOH (see also p. 304).
SOLUBILITY IN SEVERAL ALCOHOLS. (Timofeiew, 1894.)
Alcohol.
f.
Gms.
(CHCOOH)2
per 100 Gms.
Alcohol.
f
Gms.
(CHCOOH)j
per loo Gms.
Sat. Sol.
Sat. Sol.
Methyl Alcohol
22.
5
41
Propyl Alcohol
0
2O
Ethyl Alcohol
O
30.2
u
22 ,
5
24-3
u
22 .
5
34-4
Isobutyl Alcohol
0
14.2
"
22,
•5
17-5
Data for the distribution of maleic acid between ether and water at 25° are
given by Chandler, 1908.
Freezing-point data for mixtures of maleic acid and / mandelic acid are given
by Centnerszwer, 1899.
MALIC ACID I COOH.CH2CHOHCOOH.
100 gms. methyl alcohol dissolve 1 24.8 gms. malic acid at oc
167.7
91.4
54
ethyl
propyl '
dichlorethylene
trichlorethylene
0.009
O.OIO
o
15°.
15°.
(Timofeiew, 1894.)
(Wester & Bruins, 1894.)
DISTRIBUTION OF MALIC ACID BETWEEN WATER AND ETHER. (Pinnow, 1915.)
Results at 25.5°.
Gm. Mols. Acid per Liter.
Results at 15°.
Gm. Mols. Acid per Liter:
H2O Layer. Ether Layer.
0.564 0.0091
o . 288 o . 0045
O.I5I O.OO24
0.967 0.0157
Dist. Coeff.
62
64
62.9
6l.6
t2O Layer.
I.I79
0.582
Ether Layer.
0.0172
O.OO82
68.4
71
0.293
0.0040
73
0.142
0.0020
71
Freezing-point data for i malic acid -f- 1 mandelic acid are given by Cent-
nerszwer, 1899.
MALONIC ACID CH2(COOH)2.
SOLUBILITY IN WATER.
(Klobbie, 1897; Miczynski, 1886; Henry, 1884; Lamouroux, 1898, 1899.)
Gms. CH2(COOH)2 per 100.
Gms. CH2(COOH)2 per 100.
Gms. Solution.*
cc. Solution (L.).
0
52
61
10
56.5
67
20
60.5
73
25
62.2
76.3
30
64
80
40
68
86.5
t> .
Gms. Solution.*
cc. Solution (L.).
So
71
- 93
60
74-5
IOO
70
106
80
82 "
• • •
IOO
89
132 m. pt. loo
* Average curve from results of K., M., and H.
ioo gms. 95% formic acid dissolve 22.42 gms. malonic acid at 19.5°. (Aschan, 1913.)
399
MALONIC ACID
Alcohol.
Methyl Alcohol -
SOLUBILITY OF MALONIC ACID IN ALCOHOLS.
(Timofeiew, 1894.)
Gms.
A.Q OH.2(C^OOri)j Alpnhftl
^Sa^Sol!"8'
42 . 7 Ethyl Alcohol
43 . 5 Propyl Alcohol
CH,(
perioo
Ethyl Alcohol
-i5
o
+19
+19.5
-18.5
-15
o
+ 19
47-3
52.5
53-3
30
30.7
35-3
40.1
Isobutyl Alcohol
+ 19-5
-18.5
-IS
o
+19
+ 19-5
o
19
Sat. Sol.
41-3
19.5
20.2
24-3
29-5
30-7
17.5
21.2
SOLUBILITY OF MALONIC ACID IN ETHER.
(Klobbie, 1897.)
t°.
Cms. CH,(COOH).
per loo Gms.
t°.
Gms. CH2(COOH),
per 100 Gms.
Solution.
Solution.
0
6.25
30
10.5
IP
7-74
80
33
20
9
00
39
25
9-7
Gms. CH2(COOH),
t8.
per 100 Gms.
Solution.
100
46
no
56
1 20
70
132 m.
pt. 100
100 ems. saturated solution of malonic acid in pyridine contain 14.6 gms. at 26°.
(Holty, 1905.)
SOLUBILITY OF SUBSTITUTED MALONIC ACIDS IN WATER.
(Lamouroux, 1899.)
Gms. per 100 cc. Saturated Aqueous Solution.
O
15
25
30
DISTRIBUTION OF MALONIC ACID BETWEEN ETHER AND WATER AT 25°.
(Chandler, 1908.)
Mols. Acid per Liter.
Malonic
Methyl
Malonic
Ethyl
Malonic
« Propyl
Malonic
n Butyl
Malonic
Iso Amyl
Malonic
Acid.
Acid.
Acid.
Acid.
Acid.
Acid.
61.1
44-3
52.8
45-6
ii. 6
38.5
70.2
58.5
63-6
60. i
30.4
51-8
76.3
67.9
71.2
70
43-8
79-3
92.6
91.5
90.8
94-4
79-3
83-4
H2O Layer.
0.1478
O.II2I
0.0862
0.0331
MANDELIC ACID
Solvent.
Water
Ether Layer.
0.0135
O.OIO2
0.0076
O.OO27
Coef.
Cone. H2O
10.94
11.07
11.28
12.22
Dist. Coef.
corrected for
lonization.
9.86
9-79
9.86
9.82
Methyl Alcohol
« «(
Ethyl Alcohol
« «
Propyl Alcohol
« «
95% Formic Acid
C6H5.CH(OH)COOH i and d.
SOLUBILITY IN SEVERAL SOLVENTS.
t» Gms. C«H5CHOHCOOH
per iQOiGms. Sat. Sol.
15.95 (inactive acid)
19.17 (dextroacid)
5I.I (inactive acid)
20
20
O
16.5
O
16.5
o
16.5
19
64.9
46.7
53-6
35
43
40
Authority.
(Schlossberg, 1900.)
«
(Timofeiew, 1894.)
(Aschan, 1913.)
MANDELIC ACID
400
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE FOL-
LOWING MIXTURES OF MANDELIC ACID AND OTHER COMPOUNDS.
d Mandelic Acid + / Mandelic Acid
(Adrian!, 1900.)
(Centnerszwer, 1899.)
« i / « «
Methylester + I Mandelic Methylester
Isobutylester + / Mandelic Isobutylester
Acid + Dimethylpyrone
/ Menthylester + d Mandelic / Menthylester (Findky and Hickmans, 1907.
(Kendall, 1914.)
Menthyl MANDELATES.
SOLUBILITY IN ETHYL ALCOHOL.
(Findlay and Hickmans, 1909.)
Solvent. t°.
Gms.
Gms.
per 100
Solvent.
Solid
Phase.
Solvent. t°.
Gms. per 100
Gms. Solvent.
Solid
Phase.
L.
D.
L.
D.
80%
Alcohol
35
1. 08
D
80% Alcohol 10
0.287
D
«*
35
3
.19
L
IO
0-595
L
it
35
0
.80
0.80
R
IO
0.184
0.184
R
tt
35
0
•544
i-35
D+R
IO
0.404
o. 291
D+R
tt
35
2
•83
0.60
L+R
IO
0.505
0.088
L+R
"
25
0-595
D
Abs. ^
Jcohol o
1. 06
D
tt
25
I
.64
L
0
J-93
L
it
25
0
.448
0.448
R
' o
0.625
0.625
R
tt
25
o
.321
0.882
D+R
o
0-535
0.915
D+R
tt
25
I
.192
0.267
L+R
o
1.03
0-54
L+R
* d& = 0.8517.
D =1 menthyl d mandelate, [a]^17-5 = —9.45° in alcohol.
L = I menthyl / mandelate [ct]Dzo = — 140.92° in alcohol.
R = I menthyl r-mandelate [a]^11-3 = —75.03 in alcohol.
MANGANESE BORATE MnH4(BO,)2.
SOLUBILITY IN WATER AND IN AQUEOUS SALT SOLUTIONS.
(Hartley and Ramage — J. Ch. Soc. 63, 137, '93.)
per Liter in Solutions of:
f.
H20 +
trace
Na2S04.
Na2SO< Na2S04
(0.2 Gms. (20 Gms.
per Liter). per Liter).
NaCl
(20 Gms.
per Liter).
CaClj
(20 Gms.
per Liter).
14
0-94
I .7
.
. .
18
. . .
. . .
0
•77
I .31
2
.91
40
0.50
0.69(52°)
O
•65
. . .
2
•44
60
O
•36
0.6o
2
•25
80
0.08
...
0
.12
0.29
I
MANGANESE BROMIDE MnBr2.
SOLUBILITY IN WATER.
(Etard, 1894.)
t«.
Gms. MnBrj
per 100 Gms.
Solution.
Solid
Phase.
— 20
52-3 ]
SdnBra^H
— 10
O
10
54-2
56.0
57-6
M
20
25
30
59-5
60.2
61.1
M
M
t-.
Gms. MnBr3
per loo Gms.
Solution.
Solid
Phase.
40
62.8
MnBr2.4HaO
50
64.5
•
60
66.3
»
70
68.0
M
80
69.2
MnBr.2HsO
90
69.3
"
IOO
69-5
•i
us MnCl2 p
er ioo Grams
Mols. MnCJ3 Solid
per ioo Mols. H2O. Phase.
Water.
Solution.
53-8
35-o
MnCl£.4lIj
58-7
37-o
"
63-4
38.8
...
68.1
40-5
it
73-9
42-5
M
77.18
43-55
II.OS
80.71
44.68
n-55 **
88.59
46.96
12.69 "
98.15
49-53
14.05
105.4
51 .33
15.10
108.6
52.06
15-55 MnCl2.2H.
no. 6
52-52
I5-85
112.7
52.98
16.14
114.1
53-2
• . • "
iiS-3
53-5
• • • **
118.8
54-3
...
II9-5
55-o
... M
401 MANGANESE CARBONATE
MANGANESE CARBONATE MnCO8.
One liter water dissolves 5.659.io~4 mols. MnCOs = 0.065 Sm- at 25°-
(Ageno and Valla, 1911.)
MANGANESE CHLORIDE MnCl2.
SOLUBILITY IN WATER.
(Etard; Dawson and Williams — Z. physik. Chem. 31, 63, '99.)
4. • Sp. Gr. of
* • Solutions.
— 20
— 10
O
+ 10
20
25 I .4991
30 I-5049
40 L5348
50 1-5744
57.65 1.6097
60 i. 6108
70 1-6134
80
90
100
120
I4O
One liter of water dissolves 87.0 grams MnCl2. One liter of sat. HC1
dissolves 19.0 grams MnCl, at 12°. (Ditte — Compt. rend. 92, 242, '81.)
EQUILIBRIUM IN THE SYSTEM MANGANESE CHLORIDE, POTASSIUM CHLORIDE
AND WATER. (Suss, 1913.)
Cms per 100 Gnu. Gms. per 100 Gms.
f. Sat. Sol. Solid Phase. t°. Sat. Sol. Solid Phase.
MnClj. KC1. MnCl,. KC1.
6 40.23 ... MnCWHjO 52.8 50.14 6.0lMnCl2.4H2O+MnCl2.2H2O+i.i.2
6 35-94 9-41 " +I.I.2+KC1 58.3 51.72 ... MnCl2.4H2O+MnCl2.2H2O
6 ... 23.06 KC1 62.6 51.86 ... MnCl2.2H2O
28.4 44.46 ... MnClz^H-jO 62.6 49.95 6.67 " -fi.i.2
28.4 43.28 8.66 " +1.1.2 62.6 44.05 12.49 i.i.2+MnCl2.2KCl.3H2O
28.4 38.65 13.79 " +I.2.2+KC1 62.6 36,85 18.77 MnCl,.2KC1.2H2O+MnCl,.4KCl
28.4 ... 26.91 KC1 62.6 ... 31.57 KC1
1.1.2 = MnCkKC1.2H2O. 1.2.2 = MnCl22KC1.2H2O
100 cc. anhydrous hydrazine dissolve 13 gms. MnCl2 at room temp.
(Welsh and Broderson, 1915).
Fusion-point data for MnCl2 + SnCl2 (Sandonnini, 1911), MnCl2 + SnClj
(Sandonnini and Scarpa, 1911), MnCl2 + ZnCl2 (Sandonnini, 1912 and 1914).
MANGANESE CINNAMATE (C6H6CH:CHCOO)2Mn.
100 gms. H2O dissolve 0.26 gm. manganese cinnamate at 26°. (De Jong, 1909.)
MANGANESE FLUOSILICATE MnSiF6.6H2O.
100 gms. H2O dissolve 140 gms. salt at 17.5°. Sp. Gr. of solution = 1.448.
(Stolba, 1883.)
MANGANESE HYDROXIDE Mn(OH)2.
One liter H2O dissolves 2.I5.IO"6 gms. mols. Mn(OH)2 at 18°.
(Sackur and Fritzmann, 1909.)
One liter H2O dissolves 2.10.10""* gms. mols. Mn(OH2) at 18°. (Tamm, 1910.)
The determination of S. & F. was made by the neutralization method of Kuster,
that is, by determining the conductivity minimum on adding Ba(OH)2 to MnSO<
solution and calculating the Mn(OH)2 remaining in solution.
MANGANESE HYDROXIDE
402
SOLUBILITY OF MANGANESE HYDROXIDE IN AQUEOUS SOLUTIONS OF
ORGANIC SALTS.
(Tamm, 1910.)
(25 cc. of the neutral salt solution + 25 cc. of aqueous suspension of Mn(OH)»
were shaken different lengths of time. Temp, not stated.) ^
100 cc. sat. solution in I n sodium tartrate solution contain 0.052 gm.
100 cc. sat. solution in I n sodium malate solution contain 0.032 gm.
IOO cc. sat. solution in I n sodium citrate solution contain 0.095 Sm*
MANGANESE IODOMERCURATE 3MnI2.5HgI2.2oH2O.
A saturated solution of the salt in water at 17° has
1.4 MnI2.HgI2.io.22H2O and density 2.98.
MANGANESE NITRATE Mn(NO3)2.
SOLUBILITY IN WATER.
(Funk — Wiss. Abh. p. t. Reichanstalt 3, 438, 'oo.)
the composition
(Duboin, 1906.)
to
Gms. Mols.
Mn(N03)2 Mn(NO3)2 Solid
•
per loo
Gms. Sol.
per loo Phase.
Mols. H2O.
-29
42
.29
7
.37 Mn(NO3)2.6H2O.
-26
43
7
•63
— 21
44
•30
8
• O "
-16
45
•52
8
•4
- 5
48
.88
9
.61
o
50
•49
10
.2
•fn
54
•50
12
.O "
t °.
Gms.
Mn(NO3)2
Mols.
Mn(N03)2
Solid
per loo
Gms. Sol.
per loo
Mols.H2O.
Phase.
18
57-33
13.5
Mn(N03)2.6H20.
25
62.37
I6.7
"
27
65.66
19.2
Mn(N03)2.3H20.
29
66.99
2O-4
**
30
67.38
20-7
"
34
7I-31
24-9
H
35-5
76.82
33-3
M
Sp. Gr. of solution saturated at 18° = 1.624.
The Eutec is at —36° and 40.5 gms. Mn(NO3)2 per 100 gms. Sat. Sol.
MANGANESE OXALATE MnC2O4.2H2O.
SOLUBILITY IN AQUEOUS SOLUTIONS AT 25°.
(Hauser and Wirth, 1909.)
In Oxalic Acid In Ammonium Oxalate In Sulfuric Acid
Solutions. Solutions. Solutions.
Per 1000 Gms. Sat. Sol. Per 1000 Gms. Sat. Sol. Per 1000 Gms. Sat. Sol.
G. Mols.
Gms.
G.
Mols.
Gms.
Normality
Gms. Solid Phase.
(COOH)2.
Mn(COO)2.(NH<)2(COO)5
. Mn(COO)2.
H2S04.
Mn(COO)2.
O
O
.312
O,
005
O
•338
O,
025
I
.825 MnCA.2H2O
0
.0125
0
•759
0
.025
0
•479
0
.24
8
.850
0
.025
0
•930
0,
,050
0
.761
I
25
•955
0
.050
I
.080
O,
125
I
.789
2
•389
51
.080
o
•125
I
•396
O,
245
3
.970
2
.987
60
. 109 MnCA.2H20+(COOH),
0
• 25
I
.708
0,
245
4
.005
o
•952
73
.200
0
•49
2
.081
o,
,28l
4
.650
4
.500
82
.401 "
Results are also given for the solubility of MnC2O4.2H2O in aq. solutions of
H2SO4 containing also about 0.25 gm. mols. free oxalic acid per liter at 25°
MANGANESE OXIDE MnO.
Fusion-point data for mixtures of manganese oxide and silicic acid are given by
Doernickel, 1907.
MANGANESE (Hypo) PHOSPHITE Mn(PH2O2)2H2O.
100 gms. H2O dissolve 15.15 gms. salt at 25°, and 16.6 gms. at b. pt. (U. S. P.)
MANGANESE SILICATE MnSiO3.
Fusion-point data for mixtures of manganese silicate and titanate are given by
Smolensky, 1911-12.
403
MANGANESE SULFATE
MANGANESE SULFATE MnSO4.
SOLUBILITY IN WATER.
(Cottrell — J. Physic. Ch. 4, 651, '01; Richards and Fraprie — Am. Ch. J. 26, 77, *oi. The results
of Lmebarger — Am. Ch. J. 15, 225, '93, were shown to be incorrect by Cottrell, and this conclusion
was confirmed by R. and F.)
Grams MnSO4 per Grams MnSO4 per
t». zoo Gms. Solid Phase. t°. 100 Cms. Solid Phase
J Water.
Solution.
Water.
Solution.
— 10
47
.96
32
.40 MnS04.7H20
16
63
•94
38
•99
MnS044H20
0
53
•23
34
•73
18,
5
64
.19
39
.10
"
5
56
.24
35
•99
25
65
•32
39
•53
44
9
59
•33
37
.24
3°
66
•44
39
•93
'*
12
61
•77
38
.19
39
9
68
.81
40
•77
M
14-3
63
•93
39.00
49
9
72
•63
42
.08
44
5
58
.06
36
. 69 MnSO4.sH2O
41
4
60
•87
37
.84
MnSO4.H2O
9
59
.19
.18
5°
58
•17
36
.76
«
15
61
.08
37
.91
60
55
.0
35
•49
44
25
64
.78
39
.31
70
52
.0
34
.22
44
67
.76
40
.38
80
48
.0
32
•43
44
35-5
71
.61
4i
•74
90
42
•5
29
•83
44
IOO
34
.0
24
.24
44
SOLUBILITY OF MANGANESE SULFATE, COPPER SULFATE MIXED CRYSTALS
IN WATER AT 18°.
(Stortenbecker, 1900.)
Mola. per TOO Mols.
H,0.
Mol. per cent
Cuin:
Mols. per 100 Mols.
H20.
Mol. per cent
Cuin:
"Cu.
Mn. "
Solution.
Crystals.
'Cu.
Mn. "
Solution.
Crystals.
Solid Phase, CuMnSO4.sH2O,
Triclinic.
Solid Phase,
CuMnSO4.sH2O.
Triclinic.
2.282
O
IOO
IOO
[0-73
6.
37
IO
•27
10.5]
00
•5
.
.
5
.0
4.9
2.23
0-44
83
•5
0-34
7-
03
4
.60
74
.1
97
•3
.
2
•31
2-15
. i .
57
•7
95
.1
7-
375
0
.0
o.o
...
...
• o
81
•3
Solid
Phase
. CuMnSO4. Monoclinic. jH-
i-54
3-76
4.70
29
26
21
.0
.1
.8
70
•4
[1.06
5-
58
20
15
•4
•9
28.2*
23-5]
21
20
.2
• O
42
34
.6
•4
[o-73
6.
37
12
10
•45
•27
20.8
16.0]
[1.06
5-58
15
13
•9
•9
\J •
22
15
A
±8
4
0
.60
• o
5.8*
o.o
* Indicates meta stabil points.
CuMnSO4>5H2O = 100-90.8 and 2.11-0 mol. per cent Cu.
= 37.8-4.92 mol. per cent Cu.
SOLUBILITY OF MANGANESE SULFATE IN GLYCOL.
:ioo gms. saturated solution contain 0.5 gm. MnSO*-. (de Coninck, 1905.)
MANGANESE SULFATE
404
SOLUBILITY OF MANGANESE SULFATE IN AQUEOUS SOLUTIONS OF
AMMONIUM SULFATE AT 25° AND 50° AND VICE VERSA.
(Schreinemakers, 1909.)
Results at 25°.
Results at 50°.
Cms. per 100 Gins.
Sat. Sol.
MnSO4.
39.3
38.49
33.44
22.06
9.O2
2.91
1.75
1.77
O
D6 =
Solid Phase.
MnSO4.sH2O
" +D,
D,
O
3.64
4.91
9.65
20.36
37-42
42.58
43. 24
43-4
MnSO4.(NH4)2SO4.6H2O.
+(NH4)2S04
(NH4)2SO4
Gms. per
ioo Gms.
Sat
.Sol.
Solid Phase.
MnSO4.
(NH^SO,
36.26
O
, MnSd.HjO
35-35
2-95
" +DM
30.57
5-14
DM
16.86
17.62
"
6.92
35.98
"
6.29
39-71
"
5-70
43-24
3-49
44.02
(NH^O,
0
45-7
"
D2.i =
= (MnSO4
)2(NH4)2S04.
SOLUBILITY OF MANGANESE SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
SULFATE AT 35° AND VICE VERSA.
(Schreinemakers and Provije, 1913.)
Gms. per ioo Gms.
Sat. Sol.
MnSO4.
NajSO,.
39-45
0
33-92
5-23
33-06
7-97
32.92
7.42
3L05
9.20
27.67
10.76
22.14
14.28
14.58
20.01
Solid Phase.
MnSO4.HjO
+(MnS04)9.(Na2S04)IO
(MnS04)9.(Na2S04)io
Gmis. per too Gms.
Sat. Sol.
MnSO4.
Na2SO4.
13.96
21.91
12.19
22.49
10.45
23-4I
7-43
26.58
5-69
29.31
5-n
30.52
2.96
31-33
0
33
; Solid Phase.
(MnSO4)9.(NajSO4)io
+MnS04(Na2SO4),
+Na2S04
Data for the solubility of mix crystals of manganese and zinc sulfates between
o° and 39° are given by Sahmen, 1905-06.
SOLUBILITY OF MANGANESE SULFATE IN AQUEOUS ETHYL ALCOHOL.
(Schreinemakers, 1909; Schreinemakers>nd Deuse, 1912.)
. .' Results at 50°.
Gms. per ioo Gms. Sat. Sol.
MnS04.
36.26
28.12
18-75
Results at 25°.
Gms. per ioo Gms. Sat. Sol.
QHjOH. MnSO4.
O 39-3
6.8l 33-72-
liquid layers separate here
53-09 1-23
57.39 0.56
76.70 o
Solid Phase.
MnS04.SH20
MnS04.H20
C2H5OH.
O
6.67
16.02
22.63
36.47
Solid Phase.
MnS04.H;O
12-54
4.12
Composition of the liquid layers.
Water rich Layer. QH5OH rich Layer.
The following reciprocally saturated meta-
stable solutions were obtained at 50°.
Water rich Layer.
C2H5OH rich Layer.
%C2H5OH.
%MnS04.
•%QH6OH.
%MnSO4.
% C2H5OH.
% MnS04.
% C2H5OH.
% MnS04."
6.81
33-72*
53-09
1.23*
5-68
34-95
53.64
0.97
8.48
31.51
49.76
1.83
7.69
30.99
45.83
2.19
15.02
22. 6l
32.75
8.01
8.70
29.20
41-93
11.85
24.84
35-15
5-95
* These liquids in contact with MnSO4.sH2O.
Similar data are also given for 30° and for 35°. Both stable and metastable
liquid pairs were obtained at these intermediate temperatures.
Additional data for this system are also given by Cuno, 1908.
405 MANGANESE SULFATE
SOLUBILITY OF MANGANESE SULFATE IN AQUEOUS ETHYL ALCOHOL (CON.).
Composition of the conjugated liquids in contact with excess of solid salt.
C2H5OH rich Layer. Aqueous rich Layer.
%C2H5OH. % MnS04". % QHjOH. % MnSO4'.
10 37.06 5.44 13-78 25.25 MnSO4.sH2O
15 44-56 2.79 9.25 29.79
17. 47-11 2.22 8.53 30-88
21 53.55 i. 10 6.10 35.05
25 53-09 1-23 6-8i 33-72
30 45.20 2.49 8.69 30.15 MnSO4.H2O
31 43.90 2.74 8.47 30.10
35 41.71 3.44 9.24 28.61
37 38-26 4.84 11.03 26.47
41 34.01 5.86 11.93 24.97
42 32-37 6.89 13.57 23.09
43 3*-42 8.51 14.33 22.01
Data for the solubility of manganese sulfate and potassium iodate in methyl
alcohol are given by Karplus, 1907.
SOLUBILITY OF MANGANESE SULFATE IN AQUEOUS ETHYL AND PROPYL
ALCOHOL SOLUTIONS AT 20°.
(Linebarger, 1892; Snell, 1898.)
Gms. MnS04 per 100 Gms. Aq.
Ethyl Ale. Propyl Ale.
3-3 i-9
2.2 1.4
1.4 i.i
100 cc. anhydrous hydrazine dissolve about I gm. MnSO4 at room temp.
(Welsh and Broderson, 1915.)
Fusion-point data for mixtures of MnSO4 + K2SO4, and MnSO4 + Na2SO4 are
given by Calcagni and Marotta, 1914.
MANGANESE SULFIDE MnS.
One liter sat. solution in water contains 7i.6.io~6 mols. MnS = 0.00623 gm.
per liter at 18° by conductivity method. (Weigel, 1907; see also Bruner and Zawadzki, 1909.)
MANGANESE Potassium VANADATE MnKV6Oi4.8H2O.
100 gms. H2O dissolve 1.7 gms. salt at 18°. (Radan, 1889.)
MANNITOL CH2OH(CHOH)4CH2OH.
SOLUBILITY IN WATER.
(Findlay, 1902.)
to Gms. CH2OH(CHOH)4CH2OH *„ Gms. CH2OH(CHOH)4CH2OH
per roo Gms. H2O. per 100 Gms. H2O.
o 7-59 40 35-4
IO 1 1 . 63 (13-94 gms. Campetti, 1901)' $O . 8 46 . 69
2O Z7-71 (18.98 gms. Campetti, 1901) 60 6o.OI
24,5 20.96 70 74-5
30 25.4 80 91.5
35.8 29.93 I0° I33-I
100 gms. alcohol, Sp. Gr. 0.905, dissolve 1 .56 gms. mannitol at 14°. (Krusemann, 1876.)
Data for the solubility of mannitol at high pressures are given by Cohen,
Inouye and Euwen, 1910.
100 gms. sat. sol. in pyridine contain 0.47 gm. mannitol at 26°. (Holty, 1905.)
100 gms. aq. 50% pyridine dissolve 2.46 gms. mannitol at 20-25°. (Dehn, 1917.)
Data for the ternary systems mannitol -f- succinic acid nitrile -f- water and
mannitol + triethylamine + water, are given by Timmermans, 1907.
Cone, of Alcohol
Gms. MnS04 per
zoo Gms. Aq.
Cone, of Alcohol
in Wt. per cent.
Ethyl Ale.
Propyl Ale.
in Wt. per cent.
34
9-5
6
44
36
7.2
4.6
48
38
5-8
3-5
52
40
4-7
2.8
MERCURY ACETATE
406
MERCURY ACETATE (ic) Hg(C2H3O2)2, (ous) Hg2(C2H3O2)2.
100 gms. water dissolve 25 gms. mercuric acetate at 10°.
loo gms. water dissolve 0.75 gm. mercurous acetate at 13°.
loo cc. anhydrous hydrazine dissolve about 2 gms. mercurous acetate at room
temp, with precipitation of Hg. (Welsh and Broderson, 1915.)
MERCURY BENZOATE (ic) (C6H6COO)2Hg.?H2O.
100 gms. H2O dissolve 1.2 gms. mercuric benzoate at 15° and 2.5 gms. at 100°.
(Tarugiand Checchi, 1901.)
(ic) HgBr2.
SOLUBILITY IN WATER.
MERCURY BROMIDE
Q I .06 (Lassaigne, 1876.)
25 . 0.6l (SherrUl, 1903.)
ICO 2O-25 (Lassaigne.)
Mercurous bromide. One liter sat. aq. solution contains 0.000039 Sm- Hg2Bri
at 25°. (Sherrill, 1903.)
EQUILIBRIUM IN THE SYSTEM MERCURIC BROMIDE, AMMONIA, WATER AT 8°-io°.
(Gaudechon, 1910.)
The mixtures were shaken intermittently for 21-48 hrs. Both the clear sat.
solution and the separated and dried solid phases were analyzed.
Initial Mixture.
Gms. Mols. per Liter.
Sat. Solution.
Gms. Atoms, per Liter.
Solid Phase
HgBr2.
NH3.
NH«Br.
Hg.
Br.
N.
OOIIQ Jrnasc.
o,
0125
o.
0250
o
trace
0.
0154
0.0185
(NHg2Br)4HgBr2
0
0166
0.
0332
o
0.00032
0.
0172
O.O2O2
36%
" +64% NHg2BrNH4Br
o
,025
o
050
0
0.00078
0.
0241
O.O25I
NH&Br.NH^Br
0
.050
0
,100
o
0.0019
0.
0525
0.0514
o
.0125
o
,025
o.
0375
0.00178
o.
0497
0.0497
"
o
.025
o
.050
0.
075
0.0041
0.103
0.108
«
o
.0328
o
.0656
0
0984
0.0061
o.
133
0-133
93%
" +6% NHgBr.3NH4Br
0
•0365
0
•073
0
1095
0.0060
0.
132
0.133
36%
" +64% NHgBr.3NH«Br
0
.050
0
. IOO
o
150
0.007
o.
170
o. 169
NHg2Br.3NH«Br
0
. IOO
0
.200
o
.300
0.0124
o.
333
0.338
"
o
.ci8o
o
.036
o,
.01875
O.OOI
0.0315
0.0318
NHgjBr.NI^Br
0.050
0.100
0.006
0.0057
0.
1172
0.1178
"
0
.050
o
.100
o
150
0.0071
0.
169
0.168
NHg2Br.3NH4Br
0
. IOO
0
.200
o
.160
0.0083
0.
184
0.187
"
0
• 125
0
.250
o
.306
0.0160
o.
393
«
SOLUBILITY OF MERCURIC BROMIDE IN AQUEOUS SALT SOLUTIONS AT 25°.
(Herz and Paul, 1913.)
(The mixtures were constantly agitated for eight days.)
In Aq. BaBr2. In Aq. CaBr2. In Aq. KBr. In Aq. NaBr.
Mols. per Liter. Mols. per Liter. Mols. per Liter. Mols. per Liter.
In Aq. SrBr2.
Mols. per Liter.
BaBr2.
0
0.274
0.396
0-579
1.096
HgBr2.
0.017
0-370
0.540
0-759
1.478
CaBr2.
0.072
0.645
1.892
2.479
3-754
HgBr2.
o. 117
0.676
1.358
2.766
3.666
"[KBr.
0
O. 209
0.770
2.380
3-470
HgBr2.'
0.017
0.098
0.472
1.360
1.930
NaBr.
O.II8
0.596
1.142
2.448
5.246
HgBr2.
0.078
0.285
0.540
1.276
2.306
SrBr2.
0.062
0.328
0.668
1.401
1.872
HgBr2.
0.104
0.471
0.902
1.770
2.238
The following slightly higher results for KBr solutions are given by Sherrill
(1903).
Mols. KBr per liter o 0.05 o.io 0.5 0.866 234
Mols. HgBr2 per liter 0.017 O-O55 0.088 0.0359 0.611 1.407 2.096 2.339
Data for equilibrium in the system HgBr2 + KOH + H20 at 25° are given by
Herz (1910).
407
MERCURY BROMIDE
SOLUBILITY OF MERCURIC BROMIDE IN AQUEOUS SOLUTIONS OF METYHL
ALCOHOL, ETHYL ALCOHOL AND OF ETHYL ACETATE AT 25°.
(Herz and Anders, 1907.)
In Aq. Methyl Alcohol. In Aq. Ethyl Alcohol. In Aq. Ethyl Acetate.
wt. %
CH,OH
in
Sat Sr.1
Gms.
HgBr2 per
IOO CC.
Wt °7
in
. Gms. Wt. %
d»foi HgBr.perCHjCC^QHj
Sat. Sol. ioo cc. in
Solvent.
Sat. Sol.
Solvent.
Sat. Sol.
Solvent.
10.6
o
9857
0.72
O
I
.0022
0.6o
0
30.77
o
9588
1.29
20,
18
0
.9717
0.67
4
•39
47.06
o
94oi
2.52
40,
69
0
-9435
i-59
96
.76
64
o
9386
6.85
70.
01
0
.9214
6.58
IOO
78.05
o
9744
14.66
IOO
0
•9873
22.81
IOO
I,
2275
50.25
loo gms.
sat. sol. in 95%
CjHftOH
(di6 =
0.8126)
contain i
0°, 16.53
gms. at
25 and 22.63 Sms
i. at 50°.
<**50f
Sat. Sol.
I.OO22
I.OOlS
I.II59
I.OII3
Gms.
HgBr2 per
IOO CC.
Sat. Sol.
0.6o
0-574
26.69
(Reinders, 1900.)
SOLUBILITY OF MERCURIC BROMIDE IN ALCOHOLS.
(Timofeiew, 1894.)
In Methyl Alcohol. In Ethyl Alcohol. In Propyl Alcohol. In Isobutyl Alcohol
t°.
Gms. HgBr2
per ioo Gms.
t°.
Gms. HgBr2
per ioo Gms.
r.
Gms. HgBr2
per ioo Gms.
to
Gms. HgBr2
per ioo Gms.
CHjOH.
CjHsOH.
C3H7OH.
C4H,OH.
0
4LI5
0
25.2
0
14.6
o
4.6l
10
49-5
10
26.3
10
15-6
10
5^3
19
66.3
19
29.7
19
15-5
23
6.65
22
60.9
39
31-9
39
20.8
39
9-58
39
71 .3
65
44-5
65
31-3
65
15.80
65
90.8
89
66.9
86.5
42.7
97
139.1
SOLUBILITY OF MERCURIC BROMIDE IN MIXTURES OF ALCOHOLS AT 25°.
In Mixtures of Methyl
(Herz and Kuhn, 1908.)
In Mixtures of Methyl
In Mixtures of Ethyl and
and Ethyl Alcohols.
and Propyl Alcohols.
Propyl Alcohols.
% CH,OH d of
Gms.
HgBr2 per
%C,H7OH
i
f«of
Gms.
HgBr2 per
% C3H7OH
<*¥of
Gms.
HgBr2 per
Mixture. Sat- SoL
IOO CC.
Sat. Sol.
Mixture.
Sat: Sol.
IOO CC.
Sat. Sol.
Mixture.
Sat. Sol.
IOO CC.
Sat. Sol.
0 0.9873
22.8
O
I
.227
50.20
O
0.9873
22.80
4-37 0.9932
23.1
II. II
I
• 1954
47.28
8.1
o . 9802
22.25
10.4
.009
25-4
23-8
I
.1524
41-53
17-85
0.9740
21. 06
41.02
.080
33-3
65-2
I
•0257
25-30
56-6
0.9487
17.63
80.69
-185
45-7
91.8
o
•9437
16.35
88.6
0.9269
14.76
84-77
•193
46.8
93-75
o
.9368
15-86
91.2
0.9239
14.64
9I-25
.211
48.6
96.6
0
•9275
14.66
95-2
0.9227
14.06
IOO
.227
50.2
IOO
o
.9213
I3.78
IOO
0.9213
13.78
SOLUBILITY OF MERCURIC BROMIDE IN ORGANIC SOLVENTS.
In Carbon Disulfide.
(Arctowski, 1894.)
In Other Solvents at i8°-2O°.
(Sulc., 1900.)
Gms. HgBr 2
Solvent. Formula. per ioo Gms.
Solvent..
0.126
0.679
0.003
2.3I
2.34
One liter benzene dissolves 6.99 gms. HgBr2 at 25°. (Abegg and Shemll, 1903.)
Gms. HgBr2
t°. per ioo Gms. t°.
Solution.
Gms. HgBr2
per ioo Gms.
Solution.
— io 0.049 JS
0.140
— 5 0.068 20
O.l87
o 0.087 25
0.232
+ 5 °-ioS 30
0.274
10 0.122
Chloroform CHC13
Bromoform CHBr3
Carbon Tetrachloride CCU
Ethyl Bromide C2H5Br
Ethylene Dibromide
MERCURY BROMIDE 408
SOLUBILITY OF MERCURIC BROMIDE IN AN EQUIMOLECULAR MIXTURE OF
ETHYL ALCOHOL AND BENZENE. (Dukdski, 1907.)
t°. o. 10. 20. 30. 40. 50. 60.
Gms. HgBr2 per loo Gms. Sat. Sol. 10.7 12 14 16 17.5 19 21
100 gms. of sat. sol. in acetone at 25° contain 34.76 gms. HgBr2. (Reinders, 1900.)
SOLUBILITY OF MERCURIC BROMIDE IN ANILINE. (Staronka, 1910.)
Gms. Gms.
«•• g&? S?8S! So*" Phase. f- S&? SJaST "Id Phase.
C6H5NH2. C6H5NH2.
60 4 16.14 HgBr2.2C6HBNH2 IIO* 33.3 193.3 HgBr2.2C«H6NH2
70 5.8 23.83
80 8.3 35.04
QO 12.2 53.80
IOO 18.8 89.64
105 23.2 116.9
109 -7t 33-5 195 " +HgBr2.CeH6NH,
US 37.2 229.3 HgBr2.C8H6NH,
120 42.3 283.8
124 50 387.2
123 55.4 480.9
* M. pt. f Eutec.
IOO gms. ethyl acetate dissolve 13.05 gms. HgBr2 at 18°. (Naumann, 1910.)
IOO gms. methyl acetate dissolve 21.93 gms- HgBr2 at 18° (d18 sat. sol. = 1.090).
(Naumann, 1909.)
SOLUBILITY OF MERCURIC BROMIDE IN PYRIDINE. (Staronka, 1910.)
Gms. Gms.
C5HSN. C6H5N.
10 5 24 HgBr2.2CsH6N 107* 39 291 .5 HgBr-j^CsHsN+HgBrz.CjHjN
30 8 39-64 no 40.4 309 HgBrz.CjHsN
50 ii. a 57-49 " 120 45.5 381.3 "
80 17.5 96.68 I23f 50 455-8
IOO 22 128.5 I25 51 474-4 sHgBrj.aCBHjN
no 24.5 147.8 130 54.2 539.4
«8t 33-3 227-6 I34t 60 683.7
no 35.5 250.8 133 64 810.4 "
* Eutec. f m. pt.
SOLUBILITY OF MERCURIC BROMIDE IN QUINOLINE. (Staronka, 1910.)
0.0 Mol. % Gms. HgBr2 per c r j TJV,
HgBr2? loo Gms C^N. Solld Phase'
88 4.4 12.85 HgBr2.2C9H7N
in 8.9 27.28
127 14.3 46.58
134 17.6 61.16
Data for the solubility of mercuric bromide in nitrobenzene, in p nitrotoluene,
in m nitrotoluene, in o nitrotoluene and in a nitronaphthalene, determined by the
method of lowering of the freezing-point, are given by Mascarelli, 1906, and Mas-
carelli and Ascoli, 1907. Data for HgBr2 + Se are given by Olivari, 1912.
DISTRIBUTION OF MERCURIC BROMIDE BETWEEN WATER AND BENZENE
(THIOPHENE FREE) AT 25°. (Shemll, 1903.)
Mols. per Liter. Mols. per Liter.
H20 Layer. QH, Layer". H2O Layer. " C.H6 Layer.
0.017 0.194 0.876 0.00634 0.0715 0.89
0.01147 0.1303 0.88 0.00394 0.0436 0.90
0.00953 0.1074 0.89 0.00320 0.0353 °-9°
e Data are also given for the distribution between aqueous potassium iodide solu-
tions and thiophene free benzene at 25°.
Data for the solubility of mix crystals of HgBr2 -f- HgI2 in acetone at 25° and
in ethyl alcohol of di6 = 0,8126 = 95% at o°, 25° and 50° are given by Reinders
(1900). In the case of acetone, the ratio of HgBr2 in the solution increases with
increase of per cent of HgBr2 in the solid phase. In the case of the alcohol solu-
tions the ratio in solution does not show such regular variations with change of
per cent of MgBr2 in the solid phase.
409
MERCURY CHLORIDE
MERCURY CHLORIDE (ic) HgCl2, (ous) Hg2Cl2.
SOLUBILITY OF MERCURIC CHLORIDE IN WATER.
Average curve from results of Etard, 1894; Foote, 1903; Osaka, 1903-08;
Herz and Paul, 1913; Greenish and Smith, 1903; Schreinemakers and Thonus,
1912; Sherrill, 1903; Morse, 1902.
to Gms. HgCl2 per
' ioo Gms. Sat. Sol.
o 3-5
10 4.6
15-5 5-3
20 6.1
1.047)
f.
Gms. HgClj per
ioo Gms. Sat. Sol.
to Gms. HgClj per
ioo Gms. Sat. SoL
25
3°
6.9
7-7
80
IOO
23.1
38
40
60
9-3
14
120
59
78.5
20
SOLUBILITY OF MERCUROUS CHLORIDE IN WATER.
Gms. Hg2Cl2
per 100 Gms.
Sat. Sol.
Authority.
0.5 O . OOOI4O (Conductivity, Kohlrausch, 1908.)
l8 O.OOOO75 (Indirect, Behrend, 1893.)
1 8 O . OOO2 1 (Conductivity, Kohlrausch, 1908.)
0 . 000038 (Ley and Heimbucher, 1904.)
t".
Gms. Hg2Cl2
per 100 Gms.
Sat. Sol.
Authority.
24.6
O.OOO28
(Kohlrausch, 1908.)
25
0.000047
(Sherrill, 1903.)
43
O.OOO7O
(Kohlrausch, 1908.)
SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OP
SODIUM CHLORIDE.
(Homeyer and Ritsert — Pharm. Ztg. 33, 738, '88.)
Per cent Concentration 3 ^™s'
of NaCl Solutions. 'IS<>
65°
100°
0.5 10
13
44
i.o 14
18
48
5.0 30
36
64
10. o 58
68
no
25.0 120
142
196
26.0 (saturated) 128
152
208
SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OP
HYDROCHLORIC ACID AT:
o°. 20-25° (?).
(Engel — Ann. chim. phys. [6] 17, 362, '89.) (Ditte — Ibid. [5] 22, 551, '81.)
{. Mob. per
HC1.
ioo cc. Sol.
iHgCl.
Gms. pe
HC1.
r ioo cc. Sol.
HgCl2.
Sp. Gr. of
Solutions.
Farts riU
per ioo
Parts H2O.
Parts Hg(
per ioo
Parts Solu
4-3
9-7
i-57
13.11
I.II7
o.o
6.8
99
19.8
3.6l
18.04
1.238
$•«
46.8
17.8
35-5
6.49
32-44
1.427
IO.I
73-7
26.9
55-6
9.81
49.04
1.665
13-8
87.8
32-25
68.9
II .76
58.80
I .$11
21. 1
127.4
34-25
72.4
12.48
62.40
1.874
31.0
141.9
4i-5
85 5
iS-^
75-65
2.023
50.0
148.0
48.1
88 6
17-54
87.70
2.066
68.0
154.0
70-9
95-7
25.84
129.20
2.198
One liter of o.i n Hg(NO3)2 solution dissolves 105 gms. HgCl2 at 25°.
(Morse, 1902.)
This result, together with distribution experiments, show that complexes of
HgCl2 and Hg(NO3)j are formed.
MERCURY CHLORIDE
410
SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SALT SOLUTIONS AT 25°.
(Herz and Paul, 1913-)
In Aqueous Ba-
rium Chloride.
In Aqueous Cal-
cium Chloride.
In Aqueous Lith-
ium Chloride.
In Aqueous Mag-
nesium Chloride.
Mols. per Liter.
Mols. per Liter.
Mols. per Liter.
Mols.
per Liter.
1
HgCl2.
CaCl2.
HgCl2.
LiCl.
HgCl2.
MgCl2.
Hg(V
0
0.265
O
.190
0.364
0.414
0
.351
0.168
0-374
o
.385
0.697
o
,402
0.766
0.835
0
.666
0.415
0.719
0
•572
1.167
0,
656
1.108
I.27I
I
.021
o.57o
I.I3I
0
.776
1.620
o
,964
1.811
L738
I
.678
0.997
1.864
I
-336
2.645
I
429
2.645
2.265
2
.214
1.320
2.569
3
•030
5.348
I,
723
3.304
3.091
2
.896
1.728
3.206
In Aqueous Potas-
In Aqueous Sodium
In Aqueous Strontium
sium Chloride.
Chloride.
Chloride.
Mols.
per Liter.
Mols.
per Liter.
Mols. per Liter.
' KC1.
HgCl2.
' NaCl.
Hg(V
'SrCl2.
HgCl2/
O
0.265
O.20I
0.372
0.164
O
•315
O.I
0.381
(Sherrill, 1903.)
0.416
0.508
0.3II
0
.563
0.174
0-355
0.671
0.748
0.519
o
.829
0.221
0.381
I-I53
1.192
0.724
I
-342
0.25
0.542
(Sherrill, 1903.)
I.94I
2.022
1.046
I
.776
0.683
0.836
3.162
3-434
1.384
2
.293
SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AT 20° AND VICE VERSA.
(Tichomirow, 1907; see also results by Foote and Levy on next page.)
Gms. per 100 Gms. H2O.
KC1.
HgCl2. •
ouuu i lutse.
0
7-39
HgOa
1. 12
11.63
tt
2-39
15.72
tt
4-05
22.17
tt
4.84
25.16
" +2HgCl2.KCl
5.60
25-13
2 HgCl2.KCl
6.71
25.66
"
7-39
26.41
" +HgCl2.KCl
7.46
24.70
HgCl2.KCl
8.95
19-93
tt
15
22.87
"
17.57
26.12
"
Gms. per 100 Gms. H2O. - c_,: J Wl_
KC1.
HgCl2.
20-35
29 HgCl2.KCl
26.31
34.83 "
30-32
39-10 "
34-12
42.82 " +HgCl2.2KCl
34.18
39.34 HgCl2.2KCl
34-34
35-i6 "
35-54
30.63
37.72
24.3°
41-33
19.33 « +KC1
39.66
15.76 KC1
37.87
10.28 "
35-32
2.1
100 gms. i n aq. NaCl solution dissolve 25.08 gms. HgCl2 at 25°.
(Osaka, 1903-08.)
Data for the solubility of mercuric chloride in aqueous solutions of glycerol,
sucrose, tartaric and citric acids at 25° are given by Moles and Marquina, 1914.
Data for equilibrium in the system HgCl2 + KOH + H2O at 25° are given by
Herz, 1910.
Similar data for mercurous chloride + KOH + H2O at 25° are given by Herz,
1911.
411
MERCURIC CHLORIDE
SOLUBILITY OP MIXTURES OF SODIUM AND MERCURIC CHLORIDE IN
WATER AT 25°.
(Foote and Levy — Am. Ch. J. 35, 239, '06.)
Gms. per 100 Gms. Solution. Gms. per 100 Gms. Undissolved Residue.
NaCl.
HgCl2.
NaCl.
HgCl2.
H26.
26.5
none
100
none
none
18.66
51-35
. . .
16.39
... ]
18.71
21.98
...
18.64
51.42
. . .
65.42
...
18.87
51 .26
. . .
71-25
... J
14.97
57-74
16.38
74.18
9-44 '
14.03
59.69
16.36
74-21
9-43
13 .25
62 .16
16.16
74-70
9.14
13.17
62.59
15.96
74-76
9-28
12.97
62.50
78.20
...
I3-I4
62.48
. . .
88.64
. . .
62-55
90.83
• • • ,
Two determinations made at
10.3° gave:
19.46
46.49
67.46
29.19
3-35
19.48
46.50
22.83
68.85
8.32
Solid
Phase.
NaCl
NaCl and
NaCl.HgCl2.aHaO
Double Salt
NaCl.HgCl2.2H2O
Calc. Comp. = 16.01% NaCl
74-14% HgCl.g.85% HaO
and
SOLUBILITY OF MIXTURES OF POTASSIUM AND MERCURIC CHLORIDES
IN WATER AT 25°.
(Foote and Levy.)
Composition of Solution.
Grams per 100 Grams
Percentage Composition
of Undissolved
Solid
Solution.
Residue
Phase.
J KC1.
HgCl2.
KC1.
HgCl2.
H20.
26.46
none
100
none
KC1
26.24
15.04
. . .
3-63
::: i
|
26.43
15.02
. . .
26.15
... i
KC1 and
26.33
15 .02
52.01
... i
2KCl.HgCl3.H20
26-33
14.92
6 1 .04
... j
23-74
18.91
34.6l
61.66
3-731
2KCl.HgCl2.H2O
22.36
21.39
21.39
23.88
34-77
34-8o
62.02
61.84
3-2i
3-35 J
Calc. Composition
34-05% KC1, 61.84%
4.11% H20
20.32
20.26
27 .62
27.38
65-24
73-98
:::!
2KCl.HgCl2.H20 and
KCl.HgCl2.H2O
I7-85
25-34
21.89
75-io
3 -on
9.26
18.95
21 .02
73-36
5.62
iKCl.HgC!2.H2O
'6.84
19.56
22.81
20.76
20-75
73.06
74-54
6.18
4-71
Calc. Composition
20.52%KC1, 74-53% 1
4-95% H20
6.66
24.32
20.54
73-99
5-47J
'.
6.52
6.64
25.16
76.46
80.60
:::]
1 KCl.HgCl2.H2O and
KC1.2HgCl2.2H2O
I
6.27
5-77
25.11
24-73
12 .09
11.87
83.20
83.18
4-71
4-95 !
, KC1.2HgCl2.2H2O
Calc. Composition
4.68
24-75
. . .
84.46
... l
I
4.66
25-J7
. . .
93-68
I
I KCl.aHgCl2.aH30 ai
4.69
24.82
98.50
::: j
I
none
6.90
none
100. OO
none
HgCla
HgCl2,
MERCURIC CHLORIDE
412
SOLUBILITY OF MIXTURES OF MERCURIC AND RUBIDIUM CHLORIDES IN
WATER AT 25°.
(Foote and Levy, 1906.)
Composition of Solution.
Cms. per 100 Gms. Solution.
Percentage Composition of
Undissolved Residue.
Solid Phase.
RbCl.
HgCl»
RbCl.
HgCl2.
H20.
48.57
none
100
none
none Rbci
46.76
9.18
88.04
11.24.
0.72
47-54
47-55
9-49
9-39
60.33
56.59
37-51
40.75
2.16
2.66
RbCl and 2RbCl.HgCl2.H20
47-3
9-47
46.73
49-38
3-88
47-65
35 -16
iQ-35
19.58
46.50
45-98
50.92
50.80
2-58
3-22
2RbCI.HgCI2.H20 Calc. Com-
position 45-55% RbCl. 51 .05%
HgCl2.3.4% H20
34-77
19.94
43-07
52-44
4-49
2RbCl.HgCl2.H20 and 3RbCl.
34.76
20. 10
41.10
55-36
3-54
2HgCl2.2H2O
30.27
29.20
27.38
20.17
20.55
20.63
39-07
39.10
38.67
57-34
' 57'-47
57-40
3-59
3-43
3-93
3RbCl.2HgCl2.2H20
Calc. Composition
38.55% RbCl, 57.62 %HgCl2.
3.82 %H20
26.83
20.87
38.48
57-36
4.16
3RbCl.2HgCl2.2H2O and
27.09
20.97
31.40
64.35
4-25
RbCl.HgCl2.H2O
26.15
20.58
30-34
65.48
4.18
RbCl.HgCl2.H2O
23.81
18.71
30.87
65.10
4-03
Calc. Composition
18.10
14.25
29.87
65.28
4-85
29-49% RbCl, 66.11 %HgCl2,
10.87
10.42
29-33
66.15
4-52
4.40% H2O
10.68
10.56
28.59
67-99
3-42
RbCl.HgCl2.H2O and 3RbCl
10.50
10.05
26.22
72.20
1.58
4HgCl2.H20
10. 06
9.86
25.28
73-38
0.84
8.48
8.46
8.71
8.80
25-30
25-44
73-15
73-67
!-55
0.89
3RbCl.4HgCl2.H2O
Calc. Composition
24.76% RbCl, 74-01% HgCl2,
5.68
8.70
25.09
73-46
1-45
i.23%H20
5-io
8-33
24.92
73-93
i-i5
3-43
8.25
22.79
75-72
i-49
3RbCl.4HgCl2.H20 and RbCl
3-38
8
12.68
86.74
0.58
5HgCl2
2.98
7.71
8.40
91.24
1.89
1.50
7.64
7-55
8-38
8.30
. 91.78
91.81
RbCl.sHgCl2
Calc. Composition
8.20% RbCl, 91.8% HgCl,
1. 10
7.21
8.07
91.58
„ . .
0.79
0.84
7.16
7.42
6.91
2.27
93-15
97.09
...
RbCl.sHgCl2 and HgCl2
none
6.90
none
100
HgCl2
20
30
40
50
60
SOLUBILITY OF MERCURIC CHLORIDE IN ACETIC ACID.
(Etard, 1894.)
Gms. HgCU
per roo Gms.
Solution.
2-5
3-5
4-7
6
7.2
te.
70
80
90
100
Gms. HgCl2
per i oo Gms.
Solution.
8-5
9-7
ii
12.4
no
120
130
140
160
Gms. __„„,
per 100 Gms.
Solution.
I3.6
16.5
20.7
25.2
34-8
413
MERCURY CHLORIDE
SOLUBILITY OF MERCUROUS CHLORIDE (CALOMEL) IN AQUEOUS SOLUTIONS OF
SODIUM CHLORIDE, BARIUM CHLORIDE, CALCIUM CHLORIDE AND OF HYDRO-
CHLORIC ACID AT 25°.
(Richards and Archibald, 1902.)
Solid phase in each case. Calomel + about o.i gm. of mercury.
In Aqueous NaCl.
In Aqueous BaCl2.
p. Gr. of
Gms. per Liter.
Sp. Gr. of
Gms. per Liter.
olutions.
' NaCl. . HgCl.
Solutions.
BaClz. a HgCl.
. . .
5.85 O.C04I
1. 088
104.15 0.044
.040
58.50 0.041
I-I34
156.22 0.088
.078
IIQ O.I2Q
I.I74
208.30 0.107
•093
148.25 0.194
1.263
312.54 0.231
.142
222.3 0.380
.188
292.5 0.643
In Aqueous CaCl2.
In Aqueous HC1.
p. Gr. of
Gms. pe
• Liter. Sp. Gr. of
Gms. per Liter.
olutions.
' CaCl2.
HgCl. " Solutions.
HCl.j
HgCl. '
39-96
O.O22
31.69
0.034
. . .
55-5
0.033
36.46
0.048
.064
in
O.oSl
.042
95-43
0.207
.105
I38-75
0.118
.069
158-4
0-399
•151
I95-36
0.231
.091
209.2
0.548
.205
257-52
0.322
.114
267.3
0.654
•243
324.67
0.430
.119
278.7
0.675
•315
432-9
0.518 1.132
3I7-3
0.670
•358
499-5
0.510 1.153
-364-6
0.673
loo gms. bromoform, CHBr3, dissolve 0.055 8m- HgCl at i8°-2O°. (Sulc., 1900.)
SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Abe, 1912.)
'QH6OH.
HgCl2. "
ociiiu .rjua.sc.
C2H5OH.
HgCl2.
ouuu rna.be.
0
6.80
HgCk
45-84
I5-36
HgCfe
5-08
0.65
u
49.86
18.18
M
14.49
6.41
1C
53-61
21.40
(I
21
6-55
It
57.26
24.51
tt
26.25
7-31
ft
60.55
27.67
It
31-53
8.51
tf
63-95
29.86
tt
36.85
10.32
((
67-39
32.40
tt
41.36
12.64
It
SOLUBILITY OF MERCURIC CHLORIDE IN AQ. ETHYL ALCOHOL AT 25°.
(Herz and Anders, 1907.)
t. % CjHsOH
in Solvent.
dy, of Solvent.
d^ of Sat. Sol.
Gms. HgCV]
100 cc. Sat. £
0
0.9971
I-0565
7.22
20. l8
0.9665
I.02I4
6-76
40.69
0.9302
I.OlSo
10.69
70.01
0.8632
I. O6l6
23.60
100
0.7856
I.I067
36.86
MERCURY CHLORIDE
414
SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS METHYL ALCOHOL AT 25°.
(Herz and_Anders, 1907.)
Wt. % CHjOH
in Solvent.
J,« of Solvent. d^
of Sat. Sol.
Cms. HgCl2 per
100 cc. Sat. Sol.
10.60
0.9792
.0441
7.00
30-77
0.9481
.0420
11.31
37.21
0.9369
.0507
13-43
47.06
0.9186
.0809
19.71
64
0.8800
.2015
38-44
78-05
0.8489 ]
c-33*4
57-17
100
0.7879 ]
[.2160
48.62
loo cc. 90% ethyl alcohol dissolve 27.5 gms. HgCl2 at 15.5°, rfis sat. sol. = 1.065.
(Greenish and Smith, 19030
loo gms. 00.2 % ethyl alcohol dissolve 33.4 gms. HgCU at 25°. (Osaka, 1903-8.)
abs. " " " • 49.5 (de Bruyn, 1892.)
methyl
49-5
52.9
1 at 19.5° and 66.9 gms. at 25°.
(de Bruyn, 1892.)
1.2 " " at the crit. temp.
(Centnerszwer, 1910.)
SOLUBILITY OP MERCURIC CHLORIDE IN METHYL, ETHYL PROPYL,
n BUTYL, Iso BUTYL AND ALLYL ALCOHOLS.
(Etard — Ann. cliim. phys. [7] 2, 563, '94.)
NOTE. — For the solubility in Me, Et, and propyl alcohols at room
temperature, see Rohland — Z. anorg. Ch. 1-8, 328, '98; at 8.5°, 20° and
38.2°, see Timofejew — Compt. rend. 112, 1224, '91; in Me and Et
alcohols at 25°, see de Bruyn — Z. physik. Ch. 10, 783, '92. The deter-
minations of these investigators agree well with those of Etard, which
are given below.
Grams HgCl2 per 100 Grams Saturated Solution in:
fc .
CHaOH.
C2H6OH.
CsH7OH. CH3(CH2)3OH. (CH3)2CHCH2OH. CH2.CH.Cl£oH.
-30
14-5
15.0
— 20
20.1
15-7
*3-5
21.0
— 10
IS-2
26.5
I6.5
i3-7
25-5
O
20.1
29.8
17.4
14.0
5-2
30.0
+ 10
26.3
30.6
18.0
14-3
6.0
37-5
20
34-o
32.0
18.8
14.6
6.8
46-5
25
40.0
32-5
19-5
i5-S
7-2
30
44-4
33-7
20. o
16.5
7-5 '
40
58.6
35-6
23.0
19.6
9-7
60
62.5
41.2
29.8
26.5
17.0
. . .
80
66.0
47-5
36.8
33-o
24.9
100
70.1
54-3
43-8
3i-7
120
73-5
61.5
50.6
. . .
39-2
'SO
78-5
...
...
...
SOLUBILITY OF MERCURIC CHLORIDE IN AQ. ETHYL ACETATE AT 25°. ^
(Herz and Anders, 1907.) ^
Wr t. % CHjCOOCjHg j ^r c \. f
in Solvent. d*£ ol
o 0.9971
4-39*
96.76t
loot 0.884
Almost sat. with ethyl acetate. t Ethyl acetate almost sat. with H,O. J (b. pt. = 75.77°.)
t of Sat. Sol.
Gms. HgClj per
100 cc. Sat. SoL
1-0565
1.0581
7-22
7-38
I.237I
I .1126
41-55
26.42
415
MERCURY CHLORIDE
SOLUBILITY OF MERCURIC CHLORIDE IN WATER-ETHER MIXTURES AT 25°.
(Abe, 1912.)
Cms. per 100 Cms. Sat. Sol.
HgCl2.
Ether.
H2O.
ouiiu rua.sc.
6.92
87.86
5-22*
HgCl2
S-2
1.2
93-6
u
4-3
5-2
90-5
(I
2.8
5-4
91.8
tt
tt
5-4
* (Solvent, ether sat.jwith H20.)
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF ETHER AND ETHYL
ALCOHOL AT 25°. (Abe, 1912.)
Gms. per 100 Cms. Sat. Sol.
HgCl2.
32.43
35-50
37-39
37 -96
38-24
37-75
C2H6OH.
67-57
58.59
51.02
44-79
38.69
32.84
Gms. per 100 Gms. Sat. Sol.
' 5gC£ QH6OH. '
36.29 27.16
34.08 22.48
28.55 I5-2Q
20.67 8.97
5-49 o
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF ALCOHOLS AT 25°.
(Herz and Kuhn, 1908.)
In Mixtures of Ethyl and In Mixtures of Ethyl and In Mixtures of Methyl and
Methyl Alcohols. Propyl Alcohols. Propyl Alcohols.
% CH3OH
da. Of
Gms.HgCl, %C3H7OH fl
Uof
Gms. HgCl2 % C3H7OH a
' of Gms. HgCfc
in
Solvent.
Sat. Sol.
per 100 cc.
Sat. Sol.
in
Solvent.
Sat. Sol.
per too cc.
Sat. Sol.
in
Solvent.
_ TT per loo cc.
Sat. Sol. Sat. Sol.
0
I.IO7
36.86
O
I
,1070
36.86
O
I
.2l6o
48.62
4-37
I.I30
39-43
8.
i
I
,0988
36.67
II. II
I
.2278
50-34
10.40
I-I57
42.61
17-
85
I
,0857
34.06
23.80
I
.2848
57-14
41.02
1.294
58.37
56.
6
I
,0272
27.11
65.20
I
.1568
42.28
80.69
I.32I
61.67
88.
6
0
9854
21.66
91.80
I
.0090
25.09
84.77
1.288
57-82
91.
2
o
.9824
21.60
93-75
I
.0029
23-23
91-25
1.254
53.85
95-
2
o
.9772
20.87
96.6
0
.9851
21.52
100
1.216
48.62
IOO
o
,9720
20.03
IOO
0
.9720
20.03
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF ETHYL ALCOHOL AND BEN-
ZENE AND OF ETHYL ALCOHOL AND CHLOROFORM AT DIFFERENT TEMPERATURES.
(Dukelski, 1907.)
In a Mixture of
one mol. C2H6OH
+ one mol. CeHe.
Gms. HgCl2
t°. per loo Gms.
In a Mixture of In a Mixture of In a Mixture of
two mols. C2H6OH one mol. C2H6OH two mols. C2H6OH
+ one mol. CeHe. + one mol. CHsCl. + one mol. CHCla.
Gms. HgCl2 Gms. HgCl2 Gms. HgCl2
t°. per loo Gms. t°. per 100 Gms. t°. per 100 Gms.
Sat.
Sol.
Sat. Sol.
Sat. Sol.
Sat. SoL
-2.5
15
.20
-5
.2
19-45
— 20,
1 5
3-82
— 20
-5
6.60
O
15
.40
0
20.13
— 12
4-43
0
7.69
6
16
.38
9
.1
21.65
O
4-89
8
8.96
20.5
18
.40
20
•9
23-57
8
5-37
23
10.66
20.65
18
-50
24
-4
24.19
23
7.12
38
•5
12.50
' 24.5
19
•33
36
•5
26.53
38,
5
8.51
44
.2
14.40
34-5
21
•34
53
-7
31.27
44
,2
9-51
54-4
24
-84
74
38.74
45
,6
9.98
54-5
24
.42
Some of the determinations were made by the direct method of saturating the
solution at a given temperature and determining the dissolved material by evap-
orating and weighing. Others were made by the synthetic method of Alexejew.
MERCURY CHLORIDE
416
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF METHYL ALCOHOL AND
CHLOROFORM, METHYL ALCOHOL AND CARBON] TETRACHLORIDE, AND METHYL
ALCOHOL AND DICHLORETHANE AT DIFFERENT TEMPERATURES.
(Dukelski, 1907.)
In a Mixture of
one mol. CH3OH
4- one mol. CHC13.
Gms. HgClj
t°. per 100 Gms
In a Mixture of
two mols. CH3OH
+ one mol. CHC13.
Gms. HgClj
t°. per loo Gms.
In a Mixture of In a Mixture of
two mols. CH3OH two mols. CH3OH
+ one mol. CC14. + one mol. C2H4C12.
Gms. HgCl2 Gms. HgCl2
t°. per 100 Gms. t°. periooGms.
Sat. Sol.
Sat. Sol.
Sat. Sol.
Sat. Sol.
— 12
I .73
— 12
3-33
0
5-20
O
13-33
O
3-51
O
6-73
7-7
6.69
12.5
21.30
8
5-63
8
8.21
24-9
14.06
20.8
29.23
23
IO.I5
23
16.56
30.6
19.40
25-3
34.78
24.9
10.71
24-9
18.45
35-5
20.50
30.2
36.87
30.6
11.40
30.6
19.70
36.1
21. 80
37-4
37-95
38.5
12. 02
38.5
20.83
48.5
21.90
45-9
39-36
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF METHYL ALCOHOL
AND BENZENE AT DIFFERENT TEMPERATURES.
(Timofeiew, 1894.)
In a Mixture of one mol.
CH3OH + one mol. C6H6.
*'•
O
21-25
30
37
Gms. HgCl2 per roo
Gms. Sat. Sol.
8
23-9
27-3
28.1
In a Mixture of one mol.
CH3OH + two mols. C6H6.
to Gms. HgCls per 100
1 ' Gms. Sat. Sol.
O
21-25
30
37
4-8
17.1
18
18.4
SOLUBILITY OF MERCURIC CHLORIDE IN BENZENE, IN DICHLORETHANE
AND IN ETHYLACETATE AT DIFFERENT TEMPERATURES.
(Dukelski, 1907.)
In C6H6.
In C2H4C12.
f „ Gms. HgCl2 per
loo Gms. Sat. Sol.
6-5
0.26
18
o-53
34-i
0.64
54-i
i .02
69
i-39
to Gms. HgClj per
100 Gms. Sat. Sol.
O
i-33
12.5
i-55
25-3
i-73
33
2.05
45-9
2.42
In CH3COOC2H6.
xo Gms. HgClo per
* 100 Gms. Sat. Sol.
6.5
26
38
45
22.9
22.7
22.8
23-5
26.4
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF BENZENE AND ETHYL-
ACETATE, CHLOROFORM AND ETHYL ACETATE AND OF CARBO.N TETRACHLORIDE
AND ETHYL ACETATE.
(Dukelski, 1907.)
In a Mixture of one mol.
CeHe + one mol.
CH3COOC2H6.
In a Mixture of one mol.
CHCls + one mol.
CH3COOC2H5.
In a Mixture of one mol.
CCU + two mols.
CH3COOC2H6.
fo Gms. HgCl2 per
100 Gms. Sat. Sol.
O
9.62
6-5
9.62
25-7
9.78
27.6
9.98
35-5
10.81
45-3
13.69
Gms. HgCl2 per
zoo Gms. Sat. Sol.
O
26.1
36.1
46
48.5
3-34
4.07
4.78
5-38
5.10
to Gms. HgCli per
100 Gms. Sat. Sol.
O
9-24
10.3
9-05
25-7
27.6
38.5
9-32
.9-50
-9-89
45-3
11.70
417
MERCURIC CHLORIDE
SOLUBILITY OF MERCURIC CHLORIDE IN ETHYL ACETATE AND IN
ACETONE.
(Etard, 1894; von Laszcynski, 1894; Krug and McElroy, 1892; Linebarger, 1894; Aten, 1905-06.)
NOTE. — The results obtained by the above-named investigators were calcu-
lated to a common basis and plotted on cross-section paper. The variations
which were noted could not be satisfactorily harmonized, consequently all the
results are included in the following table:
SOLUBILITY.
In Ethyl Acetate.
In Acetone.
Grams HgCk per 100 Grams Solution.
Gms. HgCl2 per too Gms. Solution.
• • /
Laszcynski.
Aten. Linebarger.
Etard . K and McE . Laszcynski .
Aten.
Etard.
— 10
.
23.0
.
. .
40
... ...
44.0
*
57
.0
0
22
• O
23.2
32
.0
40
49-7
43-o
*
61
•7
+ 10
22
.2
23-5
32
•5
40
52.0 5
i.o *~5
8.9
>t 61
•7
20
22
•5
23-4
32
40
54
58.5
t
61
•7
25
22
•7
23-5
33
.0
40
37-4 55-2
S8.2
t
61
•7
30
23
.0
33
.2
40
61
•7
40
23
•5
33
•5
40
... ...
61
•7
50
24
.0
33
•5
41
... ...
.
61
•7
60
24
•7
. . .
42-5
... • * .
61
•7
80
26
.0
.
45-2
... ...
61
•7
100
. .
.
. . .
.
48.0
... ...
, »
120
.
.
50.8
...
> •
150
.
.
55-o
...
..
• •
(*)
Solid phase HgCl2(CH3)2CO.
(t) Solid Phase HgCl,.
loo gms. absolute acetone dissolve 143 gms. HgC^ at 18°.
(Naumann, 1904.)
100 gms. ethyl acetate (dig. = 0.8995) dissolve 48.8 gms. HgCl2 at 18°.
(Naumann, 1910.)
100 gms. methyl acetate (dig = 0.935) dissolve 42.6 gms. HgCl2 at 18°.
(Naumann, 1909.)
SOLUBILITY OF MERCURIC CHLORIDE IN SEVERAL SOLVENTS.
(Arctowski, 1894; von Laszcynski, 1894; Sulc, 1900.)
In Carbon Bisul-
phide (A.).
In Benzene
(von L.).
In Several Solvents
at 18-20° (S.).
Gms. HgCl2
Gms. HgCl2
Gms. HgCl2
t°.
per 100 Gms.
t°. per 100 Gms.
Solvent.
per 100 Gms.
Solution.
Solution.
Solvent.
— 10
O.OIO
15 o-537
CHBrs
0.486
o
O.OlS
41 0.616
CHC13
0.106
IO
O.O26
55 0.843
CC14
0.002
15
0.032
84 1-769
C2H5Br
2.010
20
O.O42
C2H4Br,
1-530
25
0-053
30
0.063
MERCURY CHLORIDE
418
SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF ACETONE AND BENZENE,
ETHER AND CHLOROFORM AND OF ETHYL ACETATE AND BENZENE AT 25°.
(Harden and Dover, 1917.)
In Mixtures of
CH3COCH3 + C6H6.
Gms.CH3COCHj Cms. HgCl2
per 100 Gms. per 100 Gms.
Mixture.
Mixed Solven
100
140
90
80
117
96.5
70
60
77
60
50
45
40
3i-4
30
20
20
10.7
10
0
3-9
0.66
In Mixtures of
(C2H5)20 + CHC13.
Gms. CHC13
per 100 Gms.
Mixture.
Gms. HgCl2
per 100 Gms.
Mixed Solvent.
0
IO
6-95
5-85
20
4-73
30
40
3-7°
2.80
SO
60
2.IO
I.48
70
80
QO
100
o-95
0.657
0.328
0.128
In Mixtures of
CH3COOC2H6 + C6H6.
Gms. CH3COOC2H5 Gms. HgCl2
per 100 Gms. per 100 Gms.
Mixed Solvent.
Mixture.
100
90
80
70
60
40
30
20
IO
O
49-3
26
22.1
I8.I
14.2
II
8
5-4
3-i
1.6
0.66
SOLUBILITY OF MERCURIC CHLORIDE IN BENZENE.
(Average curve from results of Linebarger, 1895; Sherrill, 1903; and Marden and Dover, 1917.)
O
10
20
Gms. HgCl2 per
zoo Gms. CaH«.
O.2O
0-39
0.56
25
30
40
Gms. HgCl2 per
100 Gms. CjHg.
0.64
0.84
SOLUBILITY OF MERCURIC CHLORIDE IN ABSOLUTE ETHYL ETHER.
(Etard, 1894; Laszcynski, 1894; Kdhler, 1879.)
fc
-2O
O
20
Gms. HgCl2 per
100 Gms. Solution.
6
6
6
60
70
80
Gms. HgCl2 per
loo Gms. Solution.
6
6-4
7
90
100
no
Gms. HgCl2 per
100 Gms. Solution.
7-5
8
8-5
SOLUBILITY OF MERCURIC CHLORIDE IN CHLORINATED HYDROCARBONS AT 25°.
(Hoffmann, Kirmreuther and Thai, 1910.)
Solvent.
Formula.
Solvent.
Gms.
HgCl2per
loo Gms.
Solvent.
Ethylene Chloride CH2C1.CH2C1 1.229 Dichlorethylene
Formula.
Tetrachlorethane C2H2Cl4
Chloroform CHCU
Pentachlorethane C2HCl6
0.090
o. 101
Trichlorethylene
Tetrachlorethylene
0.0193 Carbontetrachloride CC14
Gms.
HgCl2per
100 Gms.
Solvent.
CHC1.CHC1 0.114
CHC1.CC12 0.0274
CC12.CC12 0.0072
trace
(Aschan, 1913.)
100 gms. 95% formic acid dissolve 2.1 gm. HgCl2 at 19°.
100 gms. 95% formic acid dissolve 0.02 gm. Hg2Cl2 at 16.5°.
100 cc. anhydrous hydrazine dissolve I gm. HgCl2 with decomp. at room temp.
(Welsh and Broderson, 1915.)
loo cc. anhydrous hydrazine dissolve I gm. Hg2Cl2 with decomp. at room temp.
(Welsh and Broderson, 1915.)
IOO gms. glycerol dissolve 80 gms. HgCl2 at 25°. (Moles and Marquina, 1914.)
ioo gms. glycerol dissolve 8 gms. HgCl2 ? Hg2Cl2 at 15-16°. (Ossendowski, 1907.)
loo gms. anhydrous lanolin (m. pt. about 46°) dissolve 1.55 gms. HgCl2 at 45°.
(Klose, 1907.)
419
MERCURY CHLORINE
Gms.
SOLUBILITY OF MERCURIC CHLORIDE IN PYRIDINE.
(McBride, 1910.)
The determinations at the lower temperatures were made by stirring an excess
of HgCl2 with pyridine and analyzing the sat. solution. Those at the higher tem-
peratures were made by the synthetic method.
Cms.
*"• SPoT/ Solid Phase.
Sat. Sol.
—32.6 2.76 HgCl2.2C6HjN
— 21.75 7.86 "
0.02 13.14 "
12.58 17.34 "
18.78 19.78 "
27.23 22.65 "
31.05 24.46 "
40.90 29.29 "
50.10 34.94 "
60.03 40.36
70.15 46.44
76 ...
80.02 51.52
89 56.45
94.1 60.09
t°. Solid Phase.
Sat. Sol.
94-7 60.72 HgCl2.2CBHBN+3HgCl2.2CBH6N
74.7 48.38 HgCl2.C6H6N(unstable)
(stable)
50.53
53-41
56.45
57-84
60.72
63.06
" +HgCl2.C6H6N
HgCl2.2CBHBN (unstable)
83.5
90.4
97
IOO-5
104.2
107
106.2
95-2 60.77
106.4 61.93
109.8 62.58
114 63.18
65
69.66
(unstable)
+3HgCl2.2CsH5N
3HgCl2.2C6H6N (unstable)
" (stable)
124.2
145-5
Data for this system are also given by Staronka (1910).
Data for the solubility of HgCl2.2C6H6N and of Hg(NO3)2.2C5H6N.2H2O in
aqueous solution of pyridine at i8°.i are given by Stromholm (1908).
Data for the solubility of diamine mercuric chloride, (NH3)2HgCl2 — NH2HgCl,
in aqueous solutions of ammonia at 17.5° are given by Stromholm (1908).
SOLUBILITY OF MERCURIC CHLORIDE AND OF DOUBLE MERCURIC AND
TETRA METHYL AMINE CHLORIDE (CH3)4NC1.6HgCl2 IN AQ. ETHER
AT 1 7°. (Stromholm — J. pr. Ch. [2] 66, 443, '02; Z. physik. Chem. 44, 64, '03.)
Molecular Concentration per Liter.
Grams per Liter of Solution.
H20.
HgCl2 (*).
HgCl2 (f).
O-O
0-I5I5
0.0342
0.0656
0-1795
0-0428
0.1311
o . 2069
0-0516
0.1956
0.2339
0-0603
0.2611
o . 2489
0-0690
0.3267
o . 2849
0.0779
0.3922
0.3100
0.0866
H2O.
HgCl2 (*).
HgCl2 (f).
O
41 .16
9.26
1.18
48.64
II .60
2.36
56.08
14.00
3-52
63-38
16.34
4.70
70.16
18.70
5.88
77-20
21 .IO
7.06
84.02
23.48
(*) Results in this column are for solutions in contact with the Solid Phase HgClj. (t) Results in
this column are for solutions in contact with the Solid Phase (CH3)4NC1.6HgCl2.
SOLUBILITY OF MERCURIC CHLORIDE AND OF DOUBLE MERCURIC AND
TETRA METHYL AMINE CHLORIDE IN ALCOHOL-ETHER SOLUTIONS
AT 17
(Stromholm.)
. .
Grams CaHsOH per Liter. Grams HgCl2 (*) per Liter. Grams HgCl2 (t) per Liter.
o.o 41.16 9.26
50.00 11.87
58.76 14.38
66.96 16.90
o.o
4.58
9.16
13.74
MERCURY CHLORIDE
420
SOLUBILITY OF DOUBLE MERCURIC CHLORIDES IN AQUEOUS AND PURE
ETHER AT 16.6°.
(Stromholm, 1902, 1903.)
Mol. Cone, of HgCl2 per Liter of: Cms. HgCl2 per Liter of:
Aq.
Ether
Pure Aq. Aq. Aq. Pure Aq. Aq.
Ether. Ether Ether Ether Ether. Ether Ether
(i). (2). (3). (4). (5). (6).
0.1515 0.2387 0.2647 0.3196 41.04 64.69 71.71 86.58
0.0673 0.1157 0.1293 0.1617 18.23 3i-4i 35-05 43-79
0.0404 0.0720 0.0835 0.1034 10.95 *9 -51 22-6i 28.01
0.0342 ... 0.0706 ... 9.26 ... 19.10 ...
0.0264 ... 0.0568 ... 7.14 ... 15.39 •••
0.0209 0.0400 0.0460 0.0594 5.66 10.83 12.48 16.10
0.0063 ••• 0.0144 ••• 1-70 ... 3.90 ...
Solid Phase.
HgCl2
(CH3)4NC1.6HgCl2
(C2H5)3SC1.6HgCl2
(CH3 C2H6)2SC1.6HgClj
(CHs)2.H2NCl.2HgCl2
(i) containing 0.21055 mol. H2O per liter. (2) 0.2756 mol. H2O per liter. (3) 0.421 mol. H2O per liter.
(4) containing 3.79 gms. H2O per liter. (5) 4.97 gms. H2O per liter. (6) 7.59 gms. H2O pe
SOLUBILITY OF MIXTURES OF MERCURIC
Absolute Alcohol. (Foote, 1910.)
Gms. per 100 Gms.
Sat. Solution.
KC1.
0.21
0.28
O.22
0.28
0.25
0.17
0.38
HgCl2.
33.69
33-80
24.84
6.21
1.65
i. 57
1.03
Solid Phase.
HgCl2+5KC1.6HgCl2.2C2H6OH
sKC1.6HgCl2.2C2H5OH
7-59 gms. H2O per liter.
AND POTASSIUM CHLORIDES AT 25° IN:
Acetone. (Foote, 1910.)
Gms. per 100 Gms.
Sat. Solution.
KC1.
1.27
1-39
2-58
2.78
2-93
2.52
3-34
2.92
HgCl2.
61.87
60.68
55-85
54-41'
48.13
18.04
13.26
ii
Solid Phase.
HgCl2+KCl.sHgCl2.(CH,)2CO
KCl.5HgCl2.(CH3)2CO
+5.6.2
5.6.2
+KC1
100 gms. of sat. abs. alcohol solution
HgCl2 and 3.01 gms. NaCl at 25°.
5.6.2= 5KC1.6HgCl2.2(CH8)aCO.
of HgCl2 + NaCl contain 46.85 gms.
(Foote, 1910.)
SOLUBILITY OF MERCURIC CHLORIDE AND SODIUM CHLORIDE IN ETHYL
ACETATE AT 40°.
(Linebarger — Am. Ch. J. 16, 214, '94.)
Solid
Mols. per too Mols.
Acetate.
Gms. per too Gms.
Acetate.
Gms. per 100 Gms.
Solution.
NaCl.
HgCl2.
NaCl.
HgCl2".
NaCl.
HgCl2.
0.8
12.9
0.53
39-7
o-53
28.4
2-3
12.4
I .53
38-15
27.61
4-3
16.4
2.85
50-44
2 '.78
33-54
9.1
22.85
6.05
86.14
46.28
18.5
34-9
12.29
107.4
10-95
5J-76
20. o
40.0
13.29
123.0
II -73
55.18
HgCl3
HgCl2 + NaCl
The double salt (HgCl2)2.NaCl is formed under proper conditions.
DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND BENZENE.
(Linhart, 1915.)
Results at 40°.
Mols. HgCl2 per Liter: • Cone, in H2O
me. in C6H«
13.07
12. 08
Results at 25°.
Mols. HgCl2 per Liter; Cone, in H2O
Cone, in C6Hg
I3-65
12.91
12-35
C«Hg Layer.
O.O2IOO
O.OI224
0.005244
0.00o6l8
0.000310
0.000155
H20 Layer.
0.2866
0.15777
0.064756
0.007382
o . 003696
0.001845
11.90
11.90
C8H6 Layer.
0.02647
0.015296
0.011774
0.008041
0.004140
0.000847
H2O Layer.
0.34600
0.18470
0.138228
0.091959
o . 04586
0.009153
11.74
11.44
II. 08
I0.8I
421
MERCURY CHLORIDE
DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND ETHER.
(Hantzsch and Sebalt, 1899.)
50 cc. ether + 50 cc. sat. aqueous HgCl2 solution were shaken together at
different temperatures and after equilibrium was established the HgCl2 in each
layer determined.
I/ .
H20 Layer (cO-
(C2H5)2O Layer (<:*).
c*
0
0.0056
O.OI4O7
0.391
10
O.OO66
O.OI4I5
0.467
17-5
o . 0090
0.02150
0.419
25
O.OO95
O.O2O76
0.429
Determinations by Skinner (1892) at room temp, using concentrations of
HgCl2 in the aqueous layer varying from 1.4 to 5.9 per cent, gave a distribu-
tion coefficient, — = approximately 0.23.
DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN AQUEOUS HC1 AND ETHER
AT 18°. (Mylius, 1911.)
When I gm. of Hg as HgCl2 is dissolved in 100 cc. of H2O or aqueous HC1 and
shaken with 100 cc. of ether, the percentage of the Hg which goes into the ethe-
real layer is as follows:
Percentage Cone, of Aq. HC1 o (=H20) i 10 20
Per cent Hg in Ether Layer 69.4 13 0.4 0.2
DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND TOLUENE AT 24°.
(Brown, 1898.)
Gms. HgCJ2 per 100 cc. Cms. HgClg per TOO cc.
H2O QsHsCHs H2O
Layer. Layer. Layer.
0.442 0.0270 1.816
0.732 0.0488 3-766
0.780 0.0542 3-754
1.192 0.0812 6.688*
*.This solution saturated.
Results at Dif. Temperatures. Results at 25°.
yer.
0.130
0.292
0.298
0.528*
(Hantzsch and Vagt, 1901.)
Mols. HgCl2 per Liter:
H2O Layer fa) . C6H5CH3 Layer (<*) .
£i.
O
10
20
30
50
0.0578
0-0575
0.0576
0.0574
0.0573
o . 0047
o . 0050
0.0050
0.0051
0.0052
12.35 0.18410 0.01590 ii. 6
ii. 60 0.09193 0.00807 XI-4
11.40 0.04593 0.00410 n. i
ii. 20 0.02289 0.00211 10.8
11.25 0.01142 0.00108 10.5
0.00573 0.00057 10
Data for the effect of Hg(NO3)2 upon the distribution are given by Morse
(1902). Results for the effect of ZnCl2 are given by Drucker (1912).
FREEZING-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES:
Mercuric Chloride + Mercuric Iodide (Padoa and Tibaldi, 1903.)
+ Selenium (Olivari, 1909.)
+ Sulfur
+ Nitrobenzene (Mascarelli, 1906.)
-j- o m and p Nitrotoluene (Mascarelli, 1906, 1907, 1909.)
+ Urethan ( " 1908, 1909.)
+ a Nitronaphthalene ( " 1906, 1907.)
+ p Nitrotoluene ( " 1908.)
+ « Nitronaphthalene ( " 1906, 1907.)
+ p Nitranisole ( " 1906.)
MERCURY CINNAMATE
422
MERCURY CINNAMATE (ic) (C6H5CH.CHCOO)2Hg.?H2O.
100 gms. H2O dissolve about 0.03 gm. mercuric cinnamate at 25°. (De Jong, 1906.)
loogms. H2O dissolve about o. 53 gm. Hg cinnamateat 100°. (Tarugi& Checchi, 1901.)
MERCURIC CYANIDE
Hg(CN)2.
SOLUBILITY IN WATER.
Gms. Hg(CN), per 100:
cc. Sat. Sol."
Authonty.
Gms.H20.
— o.45Eutec. about u
13.5 9-3
15 12 . 5
2O ..."
25 ...
25 11.27
IOI.I 53-8S
One liter 5.2% aqueous NH3 solution dissolves 204.3 Sms- Hg(CN)2 at about 20°.
(Konowalow, 1898.)
SOLUBILITY OF MERCURIC CYANIDE "IN AQUEOUS POTASSIUM CYANIDE SOLU-
9-3
II. 12
IO. 95 (<Jj,£
(Guthrie, 1878.)
(Timofeiew, 1894.)
(Marsh and Struthers, 1905.)
(Konowalow, 1898, 1899.)
(Sherrill, 1903.)
(Herz and Anders, 1907.)
(Griffiths.)
TIONS AT 25
Mols per Liter.
(Sherrill, 1903.)
Gms. per Liter.
Hg(CN)2.
122.6
' KCN. Hg(CN),'. 'KCN.
0.0493 0.4855 3.21
0.0985 0.5350 6.41 135.2
O.I97O 0.6270 12.83 158.4
The regularity of the increase in solubility proves that the complex Hg(CN)j.
KCN is formed at the given concentrations.
Data are also given for the distribution of Hg(CN)2 between aqueous solu-
tions of KCN and ether at 25°.
SOLUBILITY OF MERCURIC CYANIDE IN AQUEOUS SOLUTIONS OF METHYL ALCOHOL,
(Herz and Anders, 1907.)
In Aq. Ethyl Acetate.
ETHYL ALCOHOL AND OF ETHYL ACETATE AT 25°
In Aq. Methyl Alcohol. In Aq. Ethyl Alcohol.
Wt. %
CH3OH in
Solvent.
Sat. Sol.
Gms.
Hg(CN)2
per 100 cc.
Sat. Sol.
Wt. %
C2H6OH in
Solvent.
<*«of
Sat. Sol. I
Gms.
Hg(CN)2 (
wt. %
ZHsCOOQH
8 Sat. Sol.
Gms.
Hg(CN),
oer 100 cc.
Sat. Sol.
10.6
I
.0640
11.02
0
I.
0813
10-95
O
I.oSlO
10.95
30.77
I
.0484
12.46
2O.
18
I.
0339
8.76
4-39
1.0798
10.83
47.06
I,
,0426
16.37
40.
69
I.
0006
9-O2
96.76
1-9374
2.66
64
I
.0441
20.48
70.
OI
O.
9419
9-57
IOO
0.9097
i. 80
78.05
I
.0484
24.58
IOO
0.
8552
8.19
IOO
I.
0762
34.29
SOLUBILITY OF MERCURIC CYANIDE IN ETHYL ALCOHOL, METHYL ALCOHOL
AND IN MIXTURES OF THE Two.
In Ethyl Alcohol.
(Timofeiew, '94; de Bruyn, '92;
Herz and Kuhn, 1908.)
In Methyl Alcohol.
Trwr -v
1907.)
In CH3OH+C2H6OH at 25°.
(Herz and Kuhn, 1908.)
t°.
Gms. Hg(CN)2
per loo Gms.
t°.
Gms. Hg(CN)2
per zoo Gms.
% CH3OH
in
rfj^fiOf
Gms. Hg(CN),
per loo cc.
Sat. Sol.
Sat. Sol.
Mixture.
Sat. Sol.
Sat. Sol.
0
8-3
0
26.10
4-37
0.8618
9.02
IO
8.8
14-17
29.17
10.4
0.8707
10. IO
20
9-25
23-4
32.01
41.02
0.9267
16.70
25
9-53*
27-4
31-77
80.69
1.024
28.20
30
9-8
31-7
32-53
84.77
1.034
29.60
40
10.3
38.1
33-29
91-25
1.052
30
* d.
,8=0.8552
44-5
34-05
IOO
1.076
34-30
ioo gms. of a sat. solution of Hg(CN)2 in a mixture of equimolecular amounts
of CH3OH and C6He contain 10.2 gms. Hg(CN)2 at 10°, 13 gms. at 30° and 15
gms. at 50°. (Dukelski, 1907.)
423
MERCURY CYANIDE
SOLUBILITY OF MERCURIC CYANIDE IN MIXTURES OF PROPYL AND METHYL
ALCOHOLS AND PROPYL AND ETHYL ALCOHOLS AT 25°. (Herz and Kuhn, 1908.)
In C3H7OH+CH3OH.
In C3H7OH+C2H6OH.
% C3H7OH
in Mixed
Solvent.
O
II. II
23.80
65.20
91.80
93-75
96.60
ioo
rf«of
Solvent.
0.7878
0.7894
0.7907
0.7954
0.7992
0-7995
0.7999
0.8OO4
rfyof
Sat. Sol.
I . 0760
1.0327
0.9891
0.8800
0.8376
0.8335
0.8322
0.8283
Hg(CN)2
34-3
29.52
24.48
10.48
5-04
4.23
3.98
3-44
o
8.1
I7-85
56.6
88.6
91.2
95-2
IOO
0.7867
0.7886
0.7902
0.7926
0.7973
0.7979
0.7986
0.8004
rfy Of
Sat. Sol.
0.8552
0.8549
0.8527
0.8386
0.8311
0.8306
0.8293
0.8283
Gms.
Hg(CN),
per ioo cc.
Sat. Sol.
8.91
7.90
7-30
5-21
3-87
3.84
3.64
3-44
ioo gms. propyl alcohol dissolve 3.79 gms. Hg(CN)2 at 13.5".
ioo gms. acetonitrile (b. pt. 81.6°) dissolve 9.58 gms. Hg(CN)s
(Timofeiew, 1894.)
>2 at 18°.
(Naumann and Schier, 1914.)
ioo gms. benzonitrile (b. pt. 190-1°) dissolve 1.093 Sms. Hg(CN)2 at 18°.
(Naumann, ^914.)
SOLUBILITY OF MERCURIC CYANIDE IN ANILINE. (Staronka, 1910.)
t° of Solidification
Mol. % Hg(CN)2 in sat.
Solution
41° 49 58.5 65 77 83.5 84 88.5
3.7 5.7 7.7 9 14.2 is. 2 19.7 23.4
The solid phases are the unstable Hg(CN)2.4C6H6NH2 and the stable Hg(CN)2.
2C6H6NH2 (m. pt. about 90°).
One liter sat. solution in ethyl ether contains 2.53 gms. Hg(CN)2 at 25°.
(Abegg and Sherrill, 1903.)
ioo gms. glycerol dissolve 27 gms. Hg(CN)2 at 15.5°.
SOLUBILITIES OP MERCURIC CYANIDE DOUBLE SALTS IN WATER AND
IN ALCOHOL.
Double Salt.
cold
1°
Hg(CN)2.2KCN
Hg(CN)2.2TlCN
Hg(CN)2.2TlCN 10°
2Hg(CN)2.CaBr2.5H2O cold
2Hg(CN)2.CaBr2.5H2O boiling
Hg(CN)2.KCl.H20 18°
Hg(CN)2.KBr.2H20 18°
Hg(CN)2.KBr.2H20 boiling
Hg(CN)2.BaI2.4H2O cold
Hg(CN)2.BaI2.4H2O boiling
Hg(CN)2.KI cold •
Hg(CN)2.NaI.2H2O 18°
Hg(CN)2.SrI2.6Ha6 '18°
Gms. per ioo Grams.
Water. 'Alcohol. "
22.7
12.6
9-7
100.0
400.0
14.81
7-49
ioo.o-f
6.42
250.0
6.2
22.2
50.0
IOO.O
Observer.
(Fromuller — Ber. u, oa, *78.)
14 41
(Custer.)
(Brett.)
4.42 (Custer.)
62.5 (00% Ale.)
1. 04 (34° B Ale.) (Caillot.)
15.4 (90% Ale.) (Custer.)
25.0 (90% Ale.)
14-3
SOLUBILITY OF MECURIC CYANIDE IN ORGANIC SOLVENTS AT i8°-2o°.
(Sulc, 1900.")
G. Hg(CN)2per
ioo Gms. Solvent.
0.005
O-OOI
0.013
0:001
Solvent.
Bromoform
Carbon Tetra Chloride
Ethyl Bromide
Ethylene Di Bromide
Formula.
CHBr3
CC14
C2H5Br
C2H4Br2
Data for the ternary system, mercuric cyanide, phenol, water are given by
Timmermans, 1907.
MERCURY CYANIDE
424
SOLUBILITY OF MERCURIC CYANIDE IN PYRIDINE. (Staronka, 1910.)
Mols.
t°. per foo Mols. Solid Phase.
(CN)2+
9 7-1
ii 8.7
12.2 10.4
13 II-3
13-5 12.9
14-5 13-8
16.5 15.8
20.5 15.9
Mols.
Hg(CN)
t°. per zoo M
22.5 17.3
28.5 18.4
32 19-3
38 20.6
5ls. Solid Phase.
Hg(CN),.2C8H,N
Mols.
t°. per 100 Mols. Solid Phase.
Hg(CN)2+
C5H5N
56.5 26.6 2Hg(CN)2.3C5H5N
68 27.5 Hg(CN)2.C6H6N
70 27.7
86 29
42
22.3
in
32
46
23
7
"
122.5
33
O
53
25
3
;2Hg(CN)2.3C6H5N
125
34
4
54-5
26
"
141
38
3
• O *3 'V irT ' J
100 gms. pyridine dissolve 64.8 gms. Hg(CN)2 at 18
(Schroeder, 1905.)
SOLUBILITY OF MERCURIC CYANIDE IN QUINOLINE. (Staronka, 1910.)
Mols. Hg(CN)2
per 100 Mols. Solid Phase. t°.
Hg(CN)2+C9H7N.
4.2 Hg(CN)2.3C9H7N 137
6 " tr. pt. 60° 161
89(61°) 8.2 180
99(61) 9.2 192
Mols. Hg(CN)2
> Me
Solid Phase.
45
per 100
Hg(CN)2+C9H7N.
13.2 Hg(CN)2.2C«H7N(?)
17.4
22.5
27.1 «
MERCURY FULMINATE C2HgN2O2.
One liter of solution in water contains 0.70 gm. C2HgN2O2 at 12° and 1.76
gms. at 49°. (Holleman, 1896.)
MERCURIC IODIDE HgI2.
SOLUBILITY IN WATER.
t°. Gms. HgI2 per Liter. Observer.
18 o . 0004 (conductivity method) (Kohlrausch, 1904- 05.)
17.5 0.040 (Bourgoin, 1884.)
22 0.054 (Rohland, 1898.)
25 0.0591 (Morse, 1902.)
SOLUBILITY OF MERCUROUS IODIDE IN WATER AT 25°. (Sherrill, 1903.)
One liter sat. solution contains 2 X io~7 gms. Hg2l2, determined by indirect
method.
Data for the solubility of mercurous iodide in aq. KI solutions at 25° are also
given by Sherrill.
SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS SOLUTIONS AT 25°.
(Herz and Paul, 1913.)
In Aq. Bal2.
Mols. per Liter.
'Bal^ H^lT
0.099 °-°59
0.748 0.742
0.978 0.897
1.508 1.462
In Aq. CaI2.
Mols. per Liter.
In Aq. Nal.
Mols. per Liter.
CaI2.
0-053
0.252
0.468
1.799
HgI2.
0.050
0.261
0.440
1.706
Nal.
0.794
1.385
2.225
HgI2.
0.412
0.622
0-945
In Aq. SrI2.
Mols. per Liter.
"Sr£ HgTT.
0.254 0.212
0.355 0.320
0-539 0.582
o . 608 o . 694
SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
IODIDE AT 25°. (Sherrill, 1903; Herz and Paul, 1913.)
Mols. per Liter. Gms. per Liter. Mols. per Liter. Gms. per Liter.
"KL HiiT ICL Hgi2. ' TL ' Hgi2. ' To! Hgi2. '
0.05 0.025 8.3 11.4 i 0.50 166 227.2
o.io 0.05 16.6 22.7 1.5 0.75 249 340.8
0.20 o.io 33.2 45-4 2 i 332 454.5
0.50 0.25 ' 83 113.6 2.5 1.25 415 578
Data for the distribution of mercuric iodide between aq. KI solutions and
benzene at 25° are given by Sherrill, 1903.
425 MERCURY IODIDE
EQUILIBRIUM IN THE TERNARY SYSTEM MERCURIC IODIDE, POTASSIUM
IODIDE, WATER AT 20° AND 30°. (Dunningham 1914.)
Results at 20°.
Results at 30
9
Gms. per
zoo Gms. Sat. Sol.
Gms. per
TOO Gms. Sat. Sol.
Solid PJia«a»
KI.
55*
KI.
Hgl,.
ooiiu i nase.
50-9
19.3 KI
60.6
KI
44-4
32-4
40
53
" +KHgI3
39
48
39-6
52-7
KHgla
37-4
53.6 " +KHgj3
40
52.2
"
37-8
52.6 KHglj
4O.2
51-2
"
35.1
52-2
39-3
50.3
M
35-5
512 KHgI3.H2O
33-7
49-8
"
26.7
50.3 " +UeT*
33
52
"
26.6
49-4 HgI2
3!-4
5i-7
KHglj.HzO
23-7
40 . 2 "
29.1
52.2
"
14.9
22.5
EQUILIBRIUM IN THE TERNARY SYSTEM MERCURIC IODIDE, POTASSIUM
IODIDE, ETHYL ETHER AT 20°. (Dunningham, 1914.)
Two liquid layers with compositions as follows, are formed:
Gms. per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer.
, s , " v Solid Phase.
KI. Hgl,. KI. HgI2.
i.i 2.8 None Ki+KHgS
I.I 2.4 17.6 53.2 KHgl,
0.8 2.5 16.5 56.1 HgL,
None 17 58.2 KHgi3+Hgi2
Data are also given for the four component system, HgI2 + KI + (C2H5)2O +
H2O at 20°. The results are of special interest since 3 liquid layers are formed.
SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS ETHYL ALCOHOL:
At 1 8°.'
(Bourgoin.)
(Herz and Knoch
At 25°.
— Z. anorg. Ch. 45, 266,
'05.)
Solvent.
Gms. HgI2
per Liter.
Wt.% Alcohol
in Solvent.
Hgl2 per 100 cc. Solution.
Sp. Gr. of
Solutions 25°/4°
Millimols.
Grams.
Abs. Alcohol
11.86
100
3
86
I
•754
O
•8033
H2O + 8o%
90° Ale.
2.857
95
.82
2
56
I
.162
O
.8095
H20+io%
90° Ale.
0.086
92
•44
j
,92
0
•873
0
•8154
86
•74
I
38
O
.623
O
.8300
78
•75
O
935
0
•425
O
.8465
67
•63
o-45
0
.204
0
.8721
SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS METHYL ALCOHOL AND IN
AQUEOUS ETHYL ACETATE AT 25°. (Herz and Anders, 1907.)
In Aq. Methyl Alcohol. In Aq. Ethyl Acetate.
rJS^Z0- d** of <*M of Gms" Hgl2 wt- % CHr 4« of Gms' Hgl«
CHjOH in 0 ¥ o -¥ ^ per zoo cc. COOC2H5 i8 , per 100 cc.
Solvent. SoFvent. Sat. Sol. Sat. Sol. in Solvent. Sat. Sol. Sat. Sol
47.06 0.9186 0.9187 0.044 4-36 0-9973 0-013
64 0.8800 0.8834 0.158 96.74 0.9063 1.87
78.05 0.8489 0.8519 0.445 I0° 0.9011 1.09
100 0.7879 0.8155 2.590
100 gms. sat. solution in 95% alcohol (dis = 0.8126) contain 0.72 gm. HgI2
at O°, 1. 06 gms. at 25° and 2.15 gms. at 50°. (Reinders, 1900.)
MERCURIC IODIDE
426
Alcohol.
Methyl
tt
Ethyl
Propyl
Amyl
tt
u
Isopropyl
Isobutyl
SOLUBILITY OF MERCURIC IODIDE IN ALCOHOLS.
Formula.
<in Pr nf Gms.HgI2per
*°- Solution. I??(im,s- Observer.
CHsOH
15-20
0.799
nwuuufe
3 . 24 (Rohland.)
"
19
3 • 7 (Timofeiew.)
tt
19-5
3.16 (de Bruyn.)
11
23
3 . 98 (Beckmann.)
"
66 (b. pt.)
...
6.512 (Sulc.)
CjjHsOH
15-20
O.SlO
1 . 42 (Rohland.)
tt
18
1 . 48 (Bourgoin.)
t(
19
1 . 86 (Timofeiew.)
u
19.5
....
2 . 09 (de Bruyn.)
"
25
0.803
2 . 19 (Herz and Knoch.)
u
78 (b. pt.)
.
4.325 (Sulc.)
CsH7OH
15-20
0.816
0.826 (Rohland.)
"
19
1.25 (Timofeiew.)
C&HnOH
13
0 . 66 (Laszcynski .)
tt
71
...
3-66
(i
IOO
5-30
tt
133.5
...
9-57
(CH3)2CH.OH
81 (b. pt.)
...
2.266 (Sulc.)
(CH3)2CHCH2OH
22.5
. . .
0.51 (Timofeiew.)
(i
105-107 (b.
Pt.) . . .
2-433 (Sulc.)
SOLUBILITY OF MERCURIC IODIDE IN MIXTURES OF ALCOHOLS AT 25°.
(Herz and Kuhn, 1908.)
In CH3OH+C2H6OH. In C3H7OH+CH3OH. In C3H7OH+C2H5OH.
Per cent
d of
Gms.HgI2 Percent
d of
Gms. Hglj, Percent
A__ nf Gms. Hel,
CH3OH in
Solvent.
-3L5
Sat. Sol.
per loo cc
Sat. Sol.
C3H7OH in
Solvent.
Sat. Sol.
per loo cc
Sat. Sol.
. C3H7OHin fr perioocc
Solvent. Sat- So1- Sat. Sol.
O
0.8038
I
.80
O
0.8156
3.l6
0
0
8038
.80
4
•37
0.8039
I
•93
II. II
8.1
0
8036
•73
IO
.40
0.8046
2
.08
23.80
0.8155
3.04
17-85
0
8043
•65
41
.02
0.8077
2
•32
65.20
56.6
0
8057
•55
80
.69
0.8131
2
.89
91.80
O.SlOI
i.6g
88.6
84
•77
0.8140
2
.96
93-75
O.SlIO
1.67
91.2
0
8099
.52
91
.25
0.8146
2
•98
96.60
0.8108
1-53
95-2
0
8108
• 44
IOO
0.8156
3
.16
IOO
0.8116
1.42
IOO
0
8116
.42
SOLUBILITY OF MERCURIC IODIDE IN ACETONE IN ETHYL ACETATE
AND IN BENZENE.
(Sulc; Krug and McElroy — J. Anal. Ch. 6, 186, '92; Laszcynski — Ber. 27, 2285, '94.)
In Acetone.
In Ethyl Acetate. In Benzene.
t°.
Cms. HgI2
per loo Gms.
(CH3)2CO.
Gms. HgI2
t°. per 100 Gms.
CH3COOC2H6.
I
2.83
— 20
1.49
18
3-36
+17-5
1-56
25
2.09 (K.andMcE.)
21
1.64
40
4-73
40
2.53
58
6.07
55
3-i9
56 (b.pt.) 3. 249 (Sulc.)
76
4-31
74-78 (b.pt.) 4. 20 (Sulc.)
Gms. HgI2
per loo Gms.
15 0.22
60 0.88
65 0-95
84 1.24
8o(b.pt.)o.825(SulcO
427
MERCURY IODIDE
100 gms. acetone
benzene
chloroform
acetone
dissolve 2.04 gms. HgI2 at 23°. (Beckmann and Stock, 1895.)
0.25 '
0.07
ethyl acetate
2
3-09
1.47
(red) at 25°.
(yellow) at 25°.
at 1 8°.
(Reinders, 1900.)
(Naumann, 1910.)
One liter sat. solution in benzene contains 2.24 gms. HgI2 at 25°.
(Abegg and Sherrill, 1903.)
Gms. Hglj
t°. per 100 Gms.
Aniline.
-11.48*
... c
- 6-5
23-35
+ 0-4
28.69
I7.8
42.85
21. 1
47-55
26.9
55-47
30.1
62.05
36.2
75-8o
42.9
96.49
46. 8f
SOLUBILITY OF MERCURIC IODIDE IN ANILINE.
(Pearce and Fry, 1914.)
Solid Phase.
+HgI2(red)
Gms. HgI2
t°. per zoo Gms.
Aniline.
48.8
128.1
63.6
163.8
70.82
184.1
76.2
2OI .6
95-9
246.7
io8f
"5-7
281.8
137.2
285.2
181.1
297.9
199.1
863.2
Solid Phase.
HgI2 (red)
" +HgI2 (yellow)
HgI2 (yeUow)
* Eutec.
t Tr. pt.
Additional data on this system are also given by Staronka, 1910.
Data for the solubility of mercuric iodide in nitrobenzene and in p nitrotoluene,
determined by the synthetic (sealed tube method), are given by Smits and Bak-
horst (1915). The transition point of HgI2, red to yellow, was found to be at
1.68 mol. per cent HgI2 and 127.5° m nitrobenzene and 1.81 mol. per cent HgI2
and 128° in p nitrotoluene. The interesting part of the investigation is the
characteristic prolongation of the melting line above the transition point. Similar
data for the solubility of mercuric iodide in nitrobenzene, m nitrotoluene, p nitro-
toluene and in nitronaphthalene, determined by the freezing-point method,
using a Beckmann apparatus, are given by Mascarelli (i9o6a). Observations
on the appearance and color changes of the HgI2 are given.
SOLUBILITY OF MERCURIC IODIDE IN CARBON DISULFIDE.
(Linebarger, 1894; Arctowski, 1894, 1895-96.)
116
93
86.5
10
Gms. HgI2
per 100 Gms.
Solution.
O.OI7
0.023
0.024
0.107
- 5
o
+ s
10
Gms. Hgl,
per 100 Gms.
Solution.
O.I4I
0.173 '
0.207
0.239
15
20 •
25
30
Gms. Hgl,
per 100 Gms.
Solution.
0.271
0.320
0.382
0-445
One liter sat. solution of mercuric iodide in CS-j contains 3.127 gms. at 15°
(Dawson, i
One liter sat. solution of mercuric iodide in CCU contains 0.170 gm. at 18
(Dawson, i
Data are also given by Dawson for the distribution of HgI2 between aqueous
solutions of KI and CS-j at 15° and aqueous solutions of KI and CCU at 18°.
100 cc. anhydrous hydrazine dissolve 69 gms. HgI2 with precipitation of Hg
at room temp. (Welsh and Broderson, 1915.)
MERCURY IODIDE
428
SOLUBILITY OF MERCURIC IODIDE IN SEVERAL ORGANIC SOLVENTS.
(Sulc — Z. anorg. Ch. 25, 401, 'oo.)
Solvent.
Chloroform
Chloroform
Bromoform
Tetra Chlor Methane
Tetra Chlor Methane
Ethyl Bromide
Ethyl Bromide
Ethylene Di Bromide
Ethyl Iodide
Ethylene Di Chloride
Iso Butyl Chloride
Methyl Formate
Ethyl Formate
Methyl Acetate
Acetal
Epi Chlor Hydrine
Hexane
Formula.
+ o Gms.Hgl2peric
Gms. Solvent.
CHC13
18-20
O.O4O
CHC13
61 (b. pt.)
O.l63
CHBr3
1 8-20
0.486
CC14
18-20
0.006
CC14
75 (b. pt.)
0.094
C2H5Br
18-20
0.643
C2H5Br
38° (b. pt.)
o-773
C2H4Br2
18-20
0.748
C2H5I
18-20
2.041
G.UA
8S.S0 (b. pt.)
i. 200
(CH3)0.CHCH2C1
69
0.328
HCOOCH3
36-38 "
1.166
HCOOC2H5
5^-55 "
2.150
CH3COOCH3
56-59 "
2.500
CH3CH(OC2H5)2
i°S
2.OOO
CHg.O.CH.CItjCl
117 "
6.II3
C,H14
67
0.072
SOLUBILITY OP MERCURIC IODIDE IN ETHER AND IN METHYLENB
IODIDE.
In Methylene Iodide.
In Ether.
(Sulc; Laszcynski.)
t°.
Cms. H
Cms.
o 0.62
36 0.97
35 (b.pt.) 0.47 (Sulc)
(Retgers — Z. anorg. Ch. 3, 253, '93.)
15
IOO
180
Gms. Hgl2 per i<
Cms. CH2Ia.
2-5
16.6
58.0
SOLUBILITY OF MERCURIC IODIDE IN FATTY BODIES.
(Mehu — J. pharm. chim. [5] 12, 249, '85.)
t-o Gms. HgI2 per
• ' 100 Gms. Solvent.
Solvent.
Bitter Almond Oil
Bitter Almond Oil
Castor Oil
Castor Oil
Nut Oil
25
100
25
100
ioo
1.3
4.0
20. 0
1.3
ioo grams oil of bitter almonds dissolve 5.0 grams HgI2.KI at 25°.
Solvent.
to Gms. HgI2 p
* ioo Gms. Solve
Vaseline
25
0.025
Vaseline
IOO
0.20
Poppy Oil
25
1-0
Olive Oil
25
0-4
Carbolic Acid
IOO
2-0
on.
SOLUBILITY OF MERCURIC IODIDE IN OILS.
(Anon, 1903, 1904.)
Oil
Castor
Walnut
Linseed "
Cod Liver "
Gms. Hgl,
per too cc.
Oil.
I.QO
1.29
1.23
Q-545
oa.
Peanut OU
Olive "
Almond "
Vaseline
Gms. Hglj
per IOQCC.
oa.
0.52
0.26
429 MERCURY IODIDE
SOLUBILITY OF MERCURIC IODIDE IN PYRIDINE.
(Determinations from —50° to 98.5° made by saturating the solvent at con-
stant temperatures are given by Mathews and Ritter (1917). Measurements of
the points of solidification of various mixtures of the two components, covering
the range from IO° to 135°, are given by Staronka (1910).
Cms. Hgl, Cms. HgI2
t°. per 100 Cms. Solid Phase. t°. penooGms. Solid Phase.
Sat. Sol. Sat. Sol.
— 50 1.93 HgI2.2C5H6N 90.08 61.43 Hg
-31.5 4.27 " ioo 65.72 "
'-lo 10.28 " 105 6^.89 "
. — o.i 14-85 " io7m.pt. 72.09 "
-f- 8.83 18.42 « 105 75.67 "
20.02 24.40 " ioo 79-73
25.55 27-9° " 9° 84.16 "
40.08 37-64 " 87 EutCC. 85.17 " +HgI2.C6H5N
50.02 43-15 " IOO 86 Hgl-j.CsHsN
60.07 48.29 " 120 87.16
80.05 57.60 " 135 88.78
SOLUBILITY OF MERCURIC IODIDE IN QUINOLINE.
(Staronka, 1910.)
Mols. HgI2 K Mols. HgI2'
t°. per ioo Mols. Solid Phase. t°. rper ioo Mols. " Solid Phase.
HgI2+C,H7N. HgI2+C9H7N.
IOO 4.7 ,HgI2.2C,H7N l6o 37.7 HgI2.C»H7N
115.5 9-i J65 4i-6
133-5 13-2 165 43
138 23.1 170 48.8
145 26.7 Hgi2.c,H7N 169.5 49-5
153 . 3*-4 166.5 54-4
Fusion point data for mixtures of HgI2 + I are given by Olivari, 1908.
MERCURIC IODIDE Diamine (NH3)2HgI2.
Data for the solubility of diamine mercuric iodide in aqueous ammonia solu-
tions at 20° are given by Francois (1900). The solid is not stable in solutions
containing less than 48 gms. NH3 per liter.
MERCURY NITRATE (ic) Hg(NO3)2, (oils) Hg2(NO3)2.
ioo gms. anhydrous lanolin (m. pt. about 46°) dissolve 1.15 gm. Hg(NO3)2
at 45°. (Klose, 1907.)
ioo cc. anhydrous hydrazine dissolve about 2 gms. Hg2(NO3)2 with precipita-
tion of Hg at room temp. (Welsh and Broderson, 1915.)
MERCURY OXIDE HgO.
SOLUBILITY IN WATER.
(Schick, 1903.)
t°. Gms. per 1000 cc. Solution.
25 0.0518 yellow HgO 0.0513 red HgO
ioo 0.410 yellow HgO 0.379 red HgO
At 25° the mixtures were constantly agitated for 4 days or longer. At 100°
the solutions were boiled and stirred for 5 hours. A longer period would prob-
ably have caused better agreement between the red and yellow HgO.
One liter H2O dissolves 0.05 'gm. HgO (red, large grains) at 25°. (Hulett, 1901.)
One liter H2O dissolves 0.15 gm. HgO (red, finest grains) at 25°.
MERCURY OXID.B
430
SOLUBILITY OF MERCURIC OXIDE IN AQUEOUS HYDROFLUORIC ACID AT 25°.
(Jaeger, 1901.)
Cms. Hg per
9.6 cc. Sat. Sol.
0.12 O.O242
0.24 0.0475
0.57 O.I2IO
Normality
of HF.
I. II
2.17
0.2247
0.4976
Gm. Atoms Hg
per Liter.
O.OI258
0.0247
0.0629
0.1168
0.2586
MERCURY DiPHENYL Hg(C6H5)2.
Fusion-point data for mixtures of Hg(C6H6)2 + Sn(C6H5)4 are given by Cambi
(1912).
MERCURY SELENITE HgSeO3.
SOLUBILITY IN AQUEOUS $9DiuM SELENITE SOLUTIONS AT 25°.
(Rosenheim and Pritze, 1909.)
Normality
of Na,SeOj
Solution.
0.0625
0.125
0.25
Cms. HgSeO3
per 100 Cms.
Sat. Sol.
0.18
0.32
o-53
Normality
NajSeO, of
Solution.
o-S
i
2
Cms. HgSeOj
per 100 Gms.
Sat. Sol.
0.70
1-39
2-73
MERCURY SULFATE (ic) HgSO4.
EQUILIBRIUM IN THE SYSTEM, MERCURY OXIDE, SULFUR TRIOXIDE, WATER
(Hoitsema, 1895.)
Results expressed in molecules per sum of 100 molecules of the three com-
ponents of the system. The mixtures were rotated for 3 hours or longer.
Results at 25°.
Results at 50°
H20.
S03.
HgO.
ouuu niase.
H20.
S03.
HgO.
98
•5
I
.24
o-33
3HgO.SO,
98
•9
0
.96
0
• 17
96
.6
2
•49
0.92
*
96
3
•05
o
•93
94
•4
3
•93
i.6S
"
93
.2
4
.92
I
.90
93
•9
4
.24
1 '85 I
3HgO.SOs and
92
.8
5
.10
2
.09
94
•4
4
•52
2.12)
3HgO.2SO3.2H2O
92
.8
5
.16
2
.06
93
•4
4
•65
1.94
3HgO.2SOj.2HjO
92
•5
5
•34
2
.12
92
92
•9*
•9
4
5
.81
.11
2.29
1.98
3HgO.SO,
3Hg0.2S03.2H20
92
.2
5
•57
2
.20
92
•3*
5
.20
2-54
3HgO~SO3
92
.1
5
•75
2
.11
92
•3
5
•58
2.09
3Hg0.2S03.2HjO
92
5
.80
2
.16
92
91
.1
•9
5
5
.81
•97
2.08
2.90
3HgO.S03
QI
.2*
6
•27
2
•56
QI
QI
•9
•3
6.15
6.54
2.05
2.13
3Hg0.2S03.2H20
QI
•5
6
•34
2
.19
91
.2
6
•77
2.02
HgO.SOj.HjO
QI
•3*
6
•37
2
•30
QI
•3
6
.90
1. 80
«
QI
.6
6
.69
I
•75
QI
•3
7
.67
1. 01
"
QI
.1
8.32
0
•57
QI
•3
7
.84
0.89
HgO.SO,.HjO and
90
•5
9
.11
0
•4
QI
8
•36
0.69
HgO.SO,
89
.6
10
.2
0
•23
QO
•5
8
•95
o-53
"
86
•7
13
.2
0.06
89
.2
10
.6
O.22
HgO.SO,
31
.6
68
•4
0
•03
75
.8
24
.2
trace
"
39
.2
60
•7
trace
M
.
Solid Phase.
sHgO.SO,
( 3HgO.S03 and
j 3HgO.2SOa.2HjO
3HgO.2S03.2HjO]
3HgO.SO3 and
HgO.SO,
( 3HgO.2SOj.2HjO
( and HgO.SO,
HgO.SO,
Indicates unstable equilibrium
431 MERCURY SULFATE
MERCUROUS SULFATE HglSO4.
SOLUBILITY IN WATER, IN SULFURIC ACID AND IN POTASSIUM SULFATE AT 25°.
(Drucker, 1901; Wright and Thomson, 1884-85; Wilsmore, 1900.)
Solvent. HgsSO.perLfter.
I Gm. Mol. Gms.
Water 11.71 io~4 o . 58 (o.47 w. and T., 0.39 w.)
Aq. H2SO4 ( i .96 gms. per liter) 8.31 " 0.41
Aq. H2S04 ( 4 • 90 gms. per liter) 8.78 o . 44
Aq. H2SO4 ( 9.80 gms. per liter) 8.04 0.40
Aq. K2SO4 (34-87 gms. per liter) 9 . 05 o . 45
SOLUBILITY OF MERCUROUS SULFATE IN WATER AT DIFFERENT TEMPERATURES.
(Barre, 1911.)
Gms. per 100 Gms. Sat. Sol.
Solid Phase.
Hg2S04.
16.5 o-°55 0.008
33 0.060 0.018 "
50 0.065 °-°37
75 0.074 0.063
100 0.092 0.071
The mixtures were kept at constant temp, but not constantly agitated. By
successive treatment of a given amount of Hg2SO4 with HjO, it is gradually
converted to an almost insoluble basic salt, Hg2O.Hg2SO4.H2O.
SOLUBILITY OF MERCUROUS SULFATE IN AQUEOUS POTASSIUM SULFATE
SOLUTIONS. (Barre, 1911.)
Results at 15°. Results at 33°. Results at 75°.*
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol. , Gms. per 100 Gms. Sat. Sol.
K2S04.
Hg2S04.-
H2SO4(free). K,SO4.
HgtS04. H2S04(free).
K,S04.
HfcSO*. HjSO^freej"
2.90
0.0475
O.
0080
2.94
O
.0677
0.0250
3
.10
0.1344
0.1684
5-70
0.0703
0.
0093
5-68
0
.1015
0.0350
5
•75
O.2I2O
0.2135
8.22
0.0912
0.
0098
8.30
o
.1364
0.0441
8
•So
0.2951
0.2514
8.77
0.0994
10.70
0
.1724
0.0438
13
.20
0.4610
0.2503
9-44,
'0.1080
0.
OIIO
11.90
0
.1902
0.0420
I?
•30
o . 6440
0.2225
MERCURY SULFIDE HgS.
One liter H2O dissolves 0.054 X IO"6 m°l«- HgS = 0.0000125 gm. at 18°.
(Weigel, 1906, 1907. See also Bruner and Zawadzki.)
Hexamethyl MELLITIC ACID Ester C6(COOCH3)6.
Data for the ternary system hexaniethyl mellitic acid ester, phenol and water
are given by Timmernians (1907).
MENTHOL Ci0H19OH.
One cc. of 95% alcohol dissolves about 5 gms. menthol at room temp.
(Greenish and Smith, 1903.)
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES.
Menthol + Ethylene bromide (Dahms, 1895.)
" + Menthane (Vanstone, 1909.)
" + Methyl urethan. (Scheuer, 1910.)
" -j- Naphthalene
+ p Toluidine (Pawlewiki, 1893.)
SOLIDIFICATION POINTS OF MIXTURES OF MENTHOL AND SALOL. (BeUu«ci,i9i2,i9i3.)
t° of Solidification 42 30 . 5 28 28.5 32.5 41.9
Gm. Salol per 100 Gm. Mixture 100 80 60 40 20 o
METHANE
METHANE CH4.
432
SOLUBILITY IN WATER.
(Winkler, 1901.)
t°
0.
0'.
q.
t°.
0.
0'.
q.
0
0
•05563
0.05530
0
.00396
40
0
.02369
o
.02198
0.00159
5
O
.04805
0.04764
O
.00341
50
0
.02134
0
.01876
0.00136
10
0
.04177
0.04127
0
.00296
60
o
.01954
0
.01571
O.OOII5
15
0
.03690
0.03628
O
.00260
70
0
.01825
o
.01265
0.00093
20
o
.03308,
0.03233
0
.OO232
80
0
.01770
0
.00944
0.00070
25
0
.03006
0.02913
0
.00209
90
o
•01735
0
•00535
o . 00040
30
0
.02762
0.02648
O
.00191
100
0
.01700
o
0
For the values of /3, /3' and q see Ethane, page 285.
SOLUBILITY OF METHANE IN METHYL ALCOHOL AND IN ACETONE.
(Levi, 1901, 1902.)
In methyl alcohol / (Ostwald expression, see page 227) = 0.5644 — 0.0046 / —
0.00004 f2.
In acetone / (Ostwald expression) = 0.5906 — 0.00613 t — 0.000046 P.
From which are calculated the following values:
In Methyl Alcohol. In
o 0.5644 40 0.3164 o 0.5906
10 0.5144 50 0.2344 10 0.5247
20 0.4564 60 0.1444 2° 0.4496
30 0.3904 70 0.0464 30 0.3653
SOLUBILITY OF METHANE IN SEVERAL ALCOHOLS AND
(McDaniel, 1911.)
Solvent. f. AbskCoef' Bunsen SolveQt <.„
Acetone.
40 0.2718
50 0.1691
60 0.0572
OTHER SOLVENTS.
Abs. Coef. Bunsen
A. Coef.0.
Alcohol:
Methyl (99%)
22
. i
0.4436
o.
4102
Toluene
40.
I
0
•4675
o . 4080
"
30
. 2
0.4278
o.
3883
u
So.
2
0
•4545
0.4013
"
40
0.3938
0.
3436
tt
60
0
.4502
0.3690
"
49
.8
0.2695
0.
2278
m Xylene
21.
I
0
.5146
0.4778
Ethyl (99.8%)
22
.2
0.4628
0.
4282
tt
30.
5
0
.5028
0.4529
"
30
.1
0.4503
0.
4051
tt
50
0
•4972
0.4203
n
40
0.4323
0.
3771
(l
60
0
.4870
0.3992
Isopropyl
21
• 5
0.4620
0.
4275
Hexane
22.
2
0
•6035
0.5585
"
29
•9
0.4532
o.
4081
11
40.
2
0
•5320
0.4639
"
40
0.4400
0.
3837
n
49-
7
0
.5180
0.4380
tt
60
•3
0.4244
o.
3478
"
60
0
•4964
0.4068
Amyl
22
0.4532
0.
4196
Heptane
22.
2
0
•7242
0.6720
tt
30
.1
0-4444
o.
4002
"
30.
I
0
.6906
0.6221
Benzene
22
.1
0.4954
0.
4600
11
40
0
.6675
0.5820
"
35
0.4484
0.3976
Pinene*
20
0
.4888
0.4565
"
40
. i
0.4198
0.
3661
"
30.
X
0
.4620
0.4163
"
49
•9
0-3645
0.3081 "
39-
I
0
•4472
0.3914
Toluene
25
0.4852
o.
4450
'
45
0
.4440
0.3811
"
0.4778
o.
4300
"
55-
2
0
•3694
0.3076
* b. pt. 155-160*.
Abs. coef. A = vol. of methane absorbed by unit vol.
stated.
For definition of Bunsen abs. coef. /3 see carbon dioxide,
of solvent at temp
p. 227.
433
METHANE
SOLUBILITY OF METHANE IN ETHYL ALCOHOL.
(Bunsen, 1877, 1892.)
t°. 2°. 6.4°. 11°. 15°. 19°. 23.5°.
Abs. coef. /3 (found) 0.51721 0.50382 0.49264 0.48255 0.4729 0.4629
from which the following formula was calculated.
Bunsen abs. coef. /3 for methane = 0.522745 — 0.00295882 t — 0.0000177 /*.
The solubility of methane in aq. H2SO4 (Christoff, 1906) in terms of the Ostwald
solubility expression fa. In 95.6% H2SO4, ko = 0.03303; in 61.62% H2SO4,
/2o = 0.01407; in 35. 82% H2SO4, fa = 0.01815; in H2O, /20 = 0.03756.
The solubility of methane in ethyl ether, in terms of the Ostwald Solubility
Expression / (see p. 227), is 1.066 at o° and 1.028 at 10°. (Christoff, 1912.)
The coef. of absorption /3 (Bunsen) of methane in petroleum, (Russian) is 0.144
at 10° and O.I3I at 2O°. (Gniewosz and Walfisz, 1887.)
Fusion-point data are given for diphenyl methane + naphthalene by Miolati,
(1892) and for diphenyl methane + phenol by Paterno and Ampola (1897).
Triphenyl METHANE CH(C6H6)3.
SOLUBILITY IN ANILINE.
(Hartley and Thomas, 1906.) /
By synthetic method, see page 16.
Gms.
CH(C6H5)3 Mol. per o r .
t°. per 100 cent pg££ t°
Gms. So- CH(CeHfi)3.
Gms.
CH(C6H5);
per loo
Gms. So-
* M-r Ps£
CH(C«H6)3. Pnase'
lution.
lution.
23.0
5
•4
i
•85
CH(C6H5)3.CaH6NH2
rhombs
7i
•3
67
•9
44
.6 OT<q»fcCgiNHj
35-3
9
•5
3
.8
7i
.6
71
•7
49
.1
43-o
13
•5
5
.6
M
7i
.2
76
.3
55
I "
S^-i
21
•9
9
•7
"
70
.6
78
•3
57
•9
61 .4
36
•5
.8
•I
7i
.6
82
.1
63
. 5 CH(CflH6)3 monoclinic
66.0
47
.2
25
•4
M
74
•3
84
•9
68
.2
68.7
54
.8
3i
.6
w
82
.1
9i
•7
80
•9
70.1
64
.6
40
•9
M
87
•3
96
.1
90
.2
SOLUBILITY OF TRI PHENYL METHANE IN BENZENE.
(Linebarger — Am. Ch. J. ij* 45, '93.)
Gms.
r Solid Phase.
(Hartley and Thomas.)
Gms.
Mol.
CeH6.
Solution.
3
•9
3
.90
CflH6+CH(CaH6)3.C6He 33
12
.6
4
•4
4
• o
4
.06
CH(C6H6)3.C0H6 49
•4
24
.0
8
.8
12
•5
5
.18
65
.6
38
•9
17
.2
16
.1
6
•83
73
.8
57
•5
30
.2
19
•4
7
.24
77
.1
67
•4
39
•7
23
.1
8
•95
77
•9
76
•3
So
•7
37
• 5
10
.48
(Cft?3H(cS 77
•5
80
.2
56
•4
42
.0
*9
.61
T v^rn,Mi"5/3 >
CH(CoH6)3 7°
.2
84
.1
62
.8
44
.6
22
.64
74
.6
87
•5
69
.i
5°
.1
30
.64
76
.0
89
.0
72
.2
55
•5
40
•51
78
.8
90
•5
75
•3
71
.0
140
.00
82
•3
93
.1
81
•3
76
.2
319
.67
86
.6
95
•7
87
.8
monoclinic
Hartley and Thomas call attention to the inaccuracy of Linebarger's results and
to the correctness of the determinations of Kuriloff (18973). According to
Kuriloffthetr.pt. (CeHg^CH.CeHe + C6H6 is at 4.2° and 1.25 mol. % (CeHs^CH,
the m. pt. of (C6H5)3CH.C6H6 is 78.2° and the tr. Pt.(C6H6)3CH.C6H6 + (C6H6)3.CH
is at 74° and 69.4 mol. % (C6HB)3CH. <*
Triphenyl METHANE
434
SOLUBILITY OP TRI PHENYL METHANE IN CARBON BISULPHIDE.
(Etard — Ann. chim. phys. [7] 2, 5701 '94; below — 80°, Arctowski — Z. anorg. Ch. II, 273, '95.)
40
50
60
70
So
Gms. CHCQsHs.
t°.
per 100 Gms.
Solution.
-113
•5 0-98
— 102
1.24
- 91
1.56
- 83
I.9I
- 00
3-4
t°.
Gms. CH(C6HS)3
per 100 Gms.
Solution.
-40
7-5
— 20
0
+ 10
13-7
25-8
38.7
20
43-2
30
52-9
Cms.
per 100 Gms.
Solution.
63.7
72.4
78.6
85.6
92.2
SOLUBILITY OF TRI PHENYL METHAKE rv HEXANE AND IN
CHLOROFORM. (Eurd.)
Gms. CHtCeH-Oa per 100 Gms.
Solution in:
Gms. CH(CeH5)3 per 100 Gi
Solution in:
Hexane.
Chloroform.
-So
10.5
—30
I .2
15.2
— 20
1.6
19.0
— 10
2.2
23-5
0
3-5
28.9
+ 10
5-6
35-o
20
8-3
41-5
Hezane.
Chloroform.
30
12-5
48.8
40
20. o
56.1
50
25.8
63.8
60
45-7
71.7
70
62.0
79-8
80
785
87.2
90
97.0
SOLUBILITY OF TRI PHENYL METHANE IN:
(Hartley and Thomas.)
Thiophene.
Gms. Mol.
Gms.
Pyrrole.
Mol.
to CH(QjH5)3 per Solid
' per 100 Gms. cent Phase.
Sol. CHCCeHsV
24
.6
24
•3
8
_i
29
.0
29
.8
10
.4 " fl
31
•5
33
•4
12
.1
36
.8
40
.6
J5
.8 CHCCTOs
42
•7
49
.1
20
•9 " n
46
•9
56
• 0
25
•9
53
.2
63
9
32
.8
60
• 0
72
•3
41
.8
63
9
76
•7
47
•4
68
•5
81
•9
55
.6
71
.1
84
•4
59
.8
80
.0
91
5
74
.8
89
.2
97
.6
9i
Q' M
t
o CH(C«H5)3 per Solid
* per i oo Gms. cent Phase.
Solution. CH(C6H5)3.
2f
• 7
26
.0
10
.8
CHCQHJs.C^S
*^
i
„ rhombs
33
•5
31
-I
13
•5
44
0
43
.6
21
.1
'•
47
.6
48
•4
24
•4
1C
53
-5
58
•7
32
9
••
57
•4
70
2
44
•7
•*
57
.6
74
.8
50
6
•
62
67
•7
.0
78
81
•7
9
56
60
.0
.8
CH(C«H5)3
„ monoch'nic
67
.2
82
i
6r
3
"
74
.2
87,
4
70
5
"
79
.0
90.
\J
76
3
M
87
,2
96.
2
89
9
"
F.-pt. data for triphenylmethane + naphthalene are given by Vignon (1891).
SOLUBILITY OF TRIPHENYL METHANE IN PYRIDINE. (Hartley and Thomas, 1906.)
Synthetic method used, see note, p. 16.
t
0
Gms.
CH(C,H5),
per TOO Gms,
Solution.
Mol. per
cent Solid Phase.
CH(C6H6)3.
t'
Gms.
CH(C6H5),
per TOO Gms.
Solution.
Mol. per
cent Solid Phase.
CH(C6HS)8.
22
.8
46
.2
22
CH(C6HB),
59
•3
75-6
50-3
CHCQHs),
31
•7
53
•3
27.
2 " monoclinic
67
.8
81.9
59-7
"
37
•9
57
.6
30-
7
72
.8
85-7
66.4
"
48
•7
66
.6
39-
5 "
80
.6
9i-5
77.2
(4
53
.1
70
.1
43-
5 "
86
.8
95-8
88.1
M
435
Sulfon METHANES
Ethyl and Methyl Sulfon METHANES.
SOLUBILITY IN WATER AND IN 90% ALCOHOL.
Compound. Formula. f Gms. Cmpd. per too cc.: Authority.
Water. 90% Alcohol
Sulfonal (CH3)2C(SO2C2H6)j 15.5 0.22 1.25 (Greenish and Smith, 1903.)
Tetronal (C2H5)2C(SO2C2H5)2 IS-2O O.l8 8.33 (Squire and Caines, 1905.)
Trional (CH3)(C2H6)C(SO2C2H5)2 15-20 0.31 9.0
DISTRIBUTION BETWEEN WATER AND OLIVE OIL AT ROOM TEMP.
(Baum, 1899; Meyer, 1909.)
Gms. Cmpd. per 100 cc.
Compound. Formula.
Dimethyl Sulfon Dimethyl Methane (CH3)2C(SO2.CHS)1
Diethyl Sulfon Methane
Sulfonal
Trional
Tetronal
METHYL ACETATE CH3COOCH3.
loo gms. H2O dissolve 25 gms. CH3COOCH3 at 22°.
(CHMC.HOCCSCfe.CiHs), 0.0404 0.1646
Ratio
M.
0.103
O.I5I
0.979
4.074
0.0462 0.1446 3.756
HjO Layer Oil Layer
(w) , (0) .
0.6072 O.O622
0.092
0.0686
0.610
0.070
(Traube, 1884.)
More recent data for the solubility of this compound in water are given by
(Herz, 1917).
METHYL ALCOHOL CH3OH.
FREEZING-POINTS OF MIXTURES OF METHYL ALCOHOL AND WATER.
(Pickering, 1893; Baumfi and Borowski, 1914.)
Gms.
,0
CH3OH
Solid
t .
per 100
Phase.
Gms. Sol.
— IO
14-5
Ice
— 20
25
"
-30
33
"
-40
40
"
-50
47
"
-60
52-6
Gms.
Gms.
*°
CH3OH
per loo
Gms. Sol.
Solid
Phase.
t°.
CH3OH
per loo Gms.
Mixtures.
Solid Phase.
-70
58-3
Ice
-130
75-5
Ice
-80
62.6
"
-138.5
Eutec. 77
" +CH,OH
-90
65-7
"
-130
82
CH,OH
— IOO
68.8
"
— 120
86.5
M
— no
71.5
"
— no
92
"
— 1 20
74.0
"
-95-7
IOO
"
In the vicinity of the eutectic the solutions become vitreous and direct determina-
tions of the f .-pt. cannot be made. The above results were obtained from the curve.
MISCIBILITY OF METHYL ALCOHOL (see Note, p. 287) AT o° WITH
MIXTURES OF:
Carbon Tetrachloride and Water. (Bonner, 1910.) Chloroform and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms.
00*
Gms.
H20. (
Gms.
:HSOH.
Sp. Gr. of
Mixture.
Gms.
CHC1,.
Gms.
HA
Gms.
CH,OH.
Sp. Gr. of
Mixture.
"0.935
0.015 c
).2I5
. . .
0.979
0.021
0.161
. . .
0.974
0.026 c
>.328
1.30
0.90
O.IO
0-35
•17
0.90
O.IO <
>-74
I-I3
0.80
0.2O
0.49
.12
0.80
0.20
.10
1.04
*o.73
0.27
o-57
. . .
0.70
0.30 ]
.40
I
0.70
0.30
0.60
.08
0.60
0.40 ]
.68
0.97
0.60
0.40
0.70
•05
0.50
0.50
•7i
o-9S
0.50
0.50
0.77
.02
0.40
0.60
•77
o-93
0.40
O.6O
0.83
0.20
0.80 ]
.88
0.92
0.20
0.80
0.84
0.97
O.IO
0.90 1
.90
0.92
O.IO
0.90
0.74
0.96
O.O26
0.974
•045
o-93
0.013
0.987
0.267
0.98
METHYL ALCOHOL
436
,MISCIBILITY OF METHYL ALCOHOL (see Note, p. 287) AT o° WITH
MIXTURES of:
Brombenzene and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Ethyl Bromide and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
Cms.
Cms.
Cms.
Sp. Gr. of
Gms.
Gms.
Gms.
Sp. Gr. of
C6H6Br.
H20.
CH3OH.
Mixture.
C2H5Br.
H20.
CH3OH.
Mixture.
0.991
0.009
0.230
o-973
O.O27
0.202
1.27
0.985
O.OI5
0.314
1.24
0.950
0.05
o-33
*0.98
O.O2
0.40
0.936
0.064
o-393
1.18
0.90
0.10
1. 01
1.04
0.90
O.IO
o.54
1.14
0.80
0.20
1-50
0.98
0.80.
0.20
0.86
1.05
O.yO
0.30
1.84
o-95
0.70
0.30
i .04
1. 01
0.60
0.40
2.065
0.94
0.60
0.40
1.18
o-99
0.50
0.50
2.24
0.91
0.50
0.50
1.26
0.97
0.40
O.6O
2.30
0.90
0.40
O.6O
i-3i
0.96
0.30
0.70
2.28
0.89
O.2O
0.80
I. 21
0.94
0.20
0.80
2.20
0.89
O.IO
0.90
0.94
0.94
0.095
0.905
1.927
0.90
0.022
0.978
1.94
0.98
0.016
0.984
1-332
0.91
MISCIBILITYTOF METHYL ALCOHOL (see Note, p. 287) AT o° WITH
MIXTURES OF:
Hexane and Water. (Bonner, 1910.) Heptane and Water.
Composition of Homogeneous Mixtures.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Gms.
Gms.
Gms.
Sp. Gr. of
Gms.
Gms.
Gms.
Sp. Gr. of
Hexane(i).
H20.
CH3OH.
Mixture.
Heptane(i).
H20.
CH3OH.
Mixture.
0-973
0.067
4.280
0.966
0.034
4.78
. . .
0.90
O.IO
4.69
0.80
0.90
O.IO
5-55
0.80
0.80
0.20
5.26
0.80
0-793
0.207
6.36
0.82
0.691
0.309
5-710
0.82
0.70
0.30
7-30
0.82
0.60
0.40
6.17
0.81
0.60
0.40
8.22
0.82
0.491
0.509
6.365
0.83
0.50
0.50
8.76
0.82
0.40
0.60
6.33
0.83
0.40
0.60
8.65
0.83
0.30
0.70
6.13
0.84
0.30
0.70
7.78
0.83
0.20
0.80
5-49
0.85
0.198
0.802
6.7I
0.84
O.IO
0.90
4.01
0.86
O.IO
0.90
4.40
0.87
0.016
0.984
i-759
0.91
0.038
0.962
2.96
0.91
(i) The hexane and heptane used were Kahlbaum's "aus Petroleum."
loo cc. cotton seed oil (^25 = 0.922) dissolve 4.84 gms.CK^OH at 25°.
(Wroth and Reid, 1916.)
100 cc. methyl alcohol dissolve 6.74 gms. cotton seed oil at 25°. "
DISTRIBUTION OF METHYL ALCOHOL BETWEEN" WATER AND COTTON SEED
OIL AT 25°. (Wroth and Reid, 1916.)
Oil Layer.
0.199
HjO Layer.
17.28
jxauu.
86.6
0.253
0.298
0.264
23-34
25-73
24-I5
92.2
86.2
9i-3
Gms. CHsOH per 100 cc.
Oil Layer. H2O Layer.
0.275 23.48
Q.258 24.44
0.284 23.06
Ratio.
85.2
94
81.4
Freezing-point curves (solubility, see footnote, p. i) are given for the following
mixtures: CH3OH + SO2, CH3OH + C2H5COOH, (CH3OH.HC1) +
C2H6COOH, (C2H5COOH.HC1) + CH3OH (Baume and Pamfil, 1914);
CH3OH-f NH3 (Baume and Borowski, 1914); CH3OH + CH3I (Baume and
Tykociner, 1914).
437
METHYL AMINES
METHYL AMINES CH3NH2, (CH3)2NH, (CH8)8N.
Freezing-point data (solubility, see footnote, p. i) for mixtures of CH3NH2 -f-
H2O, (CH3)2NH + H2O and (CH8)«N + H2O are given by Pickering (1893).
The solubility of methylamine and of dimethylamine in.water at 60°, calculated
from the vapor pressures determined by an aspiration method are given by Doyer
(1890) as follows:
Aminc.
CH3NH2
(CH3)2NH
Vapor Pres-
sure in
mm. Hg.
40.6
90-3
Ostwald Solu-
bility CoefJ.
(see p. 2 2 7).
5"
230
Bunsen Abs.
Coef . 0.
(see p. 227).
419
188
SOLUBILITY OF TRIMETHYL AMINE IN VARIOUS SOLVENTS AT 25°.
(v. Halban, 1913.)
The measurements were made according .to the dynamic method in the form
developed by R. Abegg and his collaborators (Gaus, 1900; Abegg and Riesenfeld,
1902). The calculations of the partial pressures of the trimethylamine were made
according to the Abegg and Riesenfeld method.
E = calc. partial pressure of (CH3)3N above a I normal solution, based on
Henry's Law.
i
}\ = solubility, i.e.. the quotient of the concentration in the solution and in the
, . mois. (CH3)3N per liter X RT X 760
gas phase: X = —, f ,~.. > ,T . ^- . Rl X 760 = 18,590.
partial pressure of (CH3)3N in mm. Hg '
Solvent. E.
Methyl Ale. 26.1
Ethyl " — -
Propyl
Amyl
Benzyl
Acetone
39-5
39-4
48-3
14.2
243
711
471
472
385
1308
76.
Solvent. E.
Acetophenone 321
Ether 349
Acetonitrile 292
Nitromethane 329
o Nitrotoluene 340
Nitrobenzene 350
x.
57-9
53-3
63-7
56.5
54-7
Solvent. E. X.
Ethyl Acetate 220 84.5
Ethyl Benzoate 244 76.2
Chloroform 31.1 598
: Bromnaphthalene 409 47
Hexane
Benzene
248
172
75
109
Two determinations are also given for triethyl amine:
X25 in hexane = 2160. X25 in nitromethane = 400.
METHYL AMINE AND TRI METHYL
Water and Amyl Alcohol.
(Herz and Fischer — Ber. 37, 4751, '04.)
Cms. NH2(CH3) Mfflimok NH2(CH3)
per ipo cc. per 10 cc.
AMINE, DISTF
Water
(Herz and Fis
Cms. N(CHa)3
per 100 cc.
Aq. Alcoholic Aq. Alcoholic
Layer. Layer. Layer. Layer.
0-37 0-12 I.I5S 0-3804
0-94 0.33 3-°36 1-070
J-57 0.54 5.054 1.759
1.89 0.69 6.083 2.219
2.00 0.72 6.429 2.315
2-53 0.92 8.126 2.981
3.30 1.24 10.613 3.974
Aq. QjHfl
Layer. Layer.
0-345 0.174
0.812 0.396
1-075 0-545
1.462 0.731
2.139 1.077
2-757 i-376
3.292 1.683
3.996 2.053
6.582 3.465
Millimok N(CHa)3
per 10 cc.
Aq.
Layer.
0.584
1-377
1.819
2.474
3.619
4-663
5-568
6.760
H-I3S
QH5
Layer.
0.295
0.670
0.921
1.237
1.823
2.328
2.847
3-474
S-86I
METHYL AMINES 438
DISTRIBUTION OF METHYLAMINE BETWEEN WATER AND CHLOROFORM AND DI-
METHYL AND TRIMETHYL AMINES BETWEEN WATER AND TOLUENE.
(Moore and Winmill, 1912.)
Results
at 1 8°.
Results
at 25°.
Results at 32.
35°.
A™;«» Gm. Equiv. per Partition
6m.
Equiv. per
Partition
Gm. Equiv. per
Partition
Amme' Liter Aq.|Layer. Coef. Liter Aq. Layer. Coef. Liter Aq. Layer.
Coef.
(CH3)NH2
0.0817
8
.496
O
. 1 2O3
7.965
0
.1399
5
•99
u
0.0809
8
•477
0
.1312
8
0
.0959
6
(CHa)2NH
0.0759
23
.28
0
.1203
19.013
0
.1003
13
.38
tt
0.0975
23
.29
O
.IOIO
19.05
O
.1043
13
•36
(CH3)3N
0.0688
3
.297
0
.0677
2.291
O
.1182
I
•815
•u
0.0791
3
.290
0
.0641
2.297
0
.1248
I
.820
Similar data for the distribution of trimethylamine between water and toluene
at 25° and at other temperatures are given by Hantzsch and Sebalt (1899) and
Hantzsch and Vagt (1901).
DiMETHYL AMINE HYDROCHLORIDE (CH,),NH.HC1.
IOO gms. H2O dissolve 369.2 gms. (CH3)2NH.HC1 at 25°. (Peddle and Turner, 1913.)
ioo gms. CHCls dissolve 16.91 gms. (CH3)2NH.HC1 at 25°.
Phenyl METHYL AMINE HYDROCHLORIDE (CH3)(C6H6)NH.HC1.
ioo gms. H2O dissolve 378.8^1113. (CH3)(C6H5)NH.HClat25°. (Peddle and Turner, '13.)
Di and TriMETHYL AMINE CHLOROPLATINATES, (CH3)2NH.H2PtCl8,
(CH3)3N.H2PtCl6.
SOLUBILITY OF EACH IN AQ. ALCOHOL AT o°. (Bertheaume, 1910.)
Gms. Each Compound (Determined Sepa-
Sol ent rately) per ioo Gms. Solvent.
(CH3)2NH.H2PtCl6. (CH3)N.H2PtClfi.
Absolute Alcohol o . 0048 o . 003 6
90° o.i 10 0.070
80° 0.325 0.243
70° 0-558 0-391
60° 0.996 0.766
METHYL BUTYRATE C3H7COOCH3.
ioo gms, H2O dissolve 1.7 gms. C3H7COOCH3 at 22°. (Traube, 1884.)
More recent data for the solubility of methyl toutyrate in water are given by
Herz, 1917.
METHYL BUTYRATE, METHYL VALERATE.
SOLUBILITY OF EACH IN AQUEOUS ALCOHOL MIXTURES.
(Bancroft, 1895; from Pfeiffer, 1892.)
ioo cc. H2O dissolve 1.15 cc. methyl butyrate at 20°.
cc. Alcohol cc. H20 Added.* <Cc. Alcohol cc. H2O Added.*
in Mixture. Butyrate. Valerate. i° Mixture. Valerate.
3 2.34 1.66 27 44.15
6 6.96 5.06 30 52.37
9 12.62 9.03 33 62.25
12 19.45 13.40 36 74.15
15 28.13 18.41 , 39 91.45
18 38.80 24 42 oo
21 55.64 30.09
24 oo 36.72
* cc. HjO added to cause the separation of a second phase in mixtures of the given amounts of ethyl
alcohol and 3 cc. portions of methyl butyrate and of methyl valerate respectively.
METHYL ETHER (CH3)20.
F.-pt. curves are given for (CH3)20 + H2O (Baume and Perrot, 1914) ; (CH3)2O -f
C2H2, (CH3)2O + SO2 (Baume, 1914); (CH3)2O + NO (Baume and Germann, 1914);
(CH3)2O + CO2 (Baume and Borowski, 1914).
439 METHYL IODIDE
METHYL IODIDE, Methylene Chloride and Methylene Bromide.
SOLUBILITY OF EACH IN WATER. (Rex, 1906.)
Gms. per 100 Gms. H2O.
CH3I. CH2C12.
o 1.565 2.363 1.173
10 1.446 2.122 1.146
20 I-4I9 2 I.I48
30 1.429 1.969 1.176
Fusion-point data for methyl iodide + pyridine are given by Aten (1905-06) A
METHYL ORANGE H2NC6H4.N2.C6H4SO3Na.
100 gms. H2O dissolve 0.02 gm. methyl orange at 20-25°.] (Dehn, 1917.)
pyridine 1.80 " "
aq. 50% pyridine 51.5
METHYL OXALATE (CH3)2C2O4.
loo gms. H2O dissolve 6.18 gms. (CH3)2C2O4 at 20-25°. (Dehn, 1917.)
pyridine "^ 4.8
aq. 50% pyridine " 93.1
95 % formic acid 22.58 at 20.2° (Aschan, 1913.)
F.-pt. data for (CH3)2C2O4 + H2O are given by Skrabal (1917).
METHYLENE BLUE (CH,),N.C.H,(NS)C.H,:N(CH,),C1.
100 gms. H2O dissolve 4.36'gms. methylene blue at*2O-25°. (Dehn, '17.)
pyridine " 0.26 "
aq. 50% pyridine 0.74
Data for the distribution of methylene blue between aniline and water are
given by Pelet-Jolivet (1909).
METHYL PROPIONATE C2H4COOCH3.
100 gms. H2O dissolve 5 gms. C2H6COOCH3 at 22°. (Traube, 1884.)
More recent data for the solubility of methyl propionate in water are given by
Herz (1917).
METHYL SALICYLATE C6H4OH.COOCH3.
100 cc. H2O dissolve 0.074 Sm- C6H4OH.COOCH3 at 30°. (Gibbs, 1908.)
100 cc. o.i n H2SO4 dissolve 0.077 gm. C6H4OH.COOCH3 at 30°.
SOLUBILITY OF METHYL SAHCYLATE IN AQUEOUS ALCOHOL AT 25°. (Seidell, 1910.)
Wt. %
C2H5OH
in Solvent.
<*«of
Sat. Sol.
Gms. CgHjiOH.-
COOCH3 per
loo Gms. Sat. Sol.
Wt. %
in Solvent.
<*25 Of
Sat. Sol.
Gms. C6H4OH.-
COOCH3 per
0
I
0.12
60
0.923
° iT.oo' °
30
0.958
O.6O
65
0.929
30.50
40
0.940
2.30
70
0-943
39-40
50
0.925
6. 20
75
0-974
58.50
55
0.922
10
80
1.050
72
SOLUBILITY OF METHYL SALICYLATE IN AQUEOUS ALCOHOL AT DIFFERENT
TEMPERATURES. (Seidell, 1910.)
Wt. % C2HSOH Gms. QI^OH.COOCHs per 100 cc. Solvent at:
in Solvent.
O
30
40
50
55
60
65
70
75
80
15°.
20°.
25°.
30°.
(about) o.i
O.I
O.I
O.I
0.3
0.4
0.5
0.6
0.8
1 .1
1.8
2.4
3-5
5
6
4.2
6
7-8
9-5
7-7
10
12.5
15-5
13
16.5
20.2
24.5
22
28
33
40
43
52
62
72
92
135
180
230
METHYL StTLFATE 440
METHYL SULFATE (CH,)2SO4.
RECIPROCAL SOLUBILITY OF METHYL SULFATE AND OIL OF TURPENTINE.
The determinations were made by the synthetic method (sealed tubes).
The dz5 of the oil of turpentine, CioHie, was 0.8602, its absolute index of refraction
for yellow light at 25° was 1.467 and its rotation in a loo-mm. tube was —32.25°.
Cms. (CH3)2S04 per 100 Gms. Gms. (CH3)2SO4 per 100 Cms.
t°. (CH3)2S04 CwHw, . ' (CH3)jS04 C10H16 '
Rich Layer. Rich Layer. Rich Layer. Rich Layer.
30 95 4 80 87 13
40 93 5 90 84 17
50 92 6 ico 76 27
60 91 8 105 68 37
70 89 10 108 . 2 (crit. t.) 50 . 5
The results are influenced appreciably by the age and purity of the products
and by the length of time the mixtures are kept in the sealed tubes. Somewhat
different results were obtained with a sample of turpentine containing 5 vol. % of
white spirit.
MICHLER'S KETONE (Tetramethyl-pa-diamidobenzophenone) CO[C6H4(4)-
N(CH3)2]2.
100 gms. H2O dissolve 0.04 gm. of ketone at 20-25°. (Dehn, 1917 )
pyridine* " 9.92 "
aq. 50% pyridine " 3-59 "
MOLYBDENUM TRIOXIDE (Molybdic acid dihydrate) MoO3.2H2O.
SOLUBILITY IN WATER. (Rosenheim and Bertheim, 1903.)
Gms. MoO3 per 1000 Gms. Gms. MoO3 per 1000 Gms.
Sat. Solution. H2O.
18 1-065 i. 066 59
23 1.822 1.856 60
30 2.570 2.638 66
40 4.541 4.761 70
48 5.980 6.360 74.4
50.2 6.431 6.873 75
54 7.283 7.855 79
When a solution of the dihydrate is held at 40-50°, considerable amounts of crys-
tals, designated by the authors as a molybdic acid monohydrate, separate. They
differ from the /8 molybdic acid monohydrate obtained by direct conversion of the
dihydrate at 70°, in being better crystals and in yielding solutions which can be
filtered.
SOLUBILITY OF a MOLYBDIC ACID MONOHYDRATE IN WATER.
(Rosenheim and Davidsohn, 1903.)
Gms. MoO3 per 1000 Gms. Gms. MoO3 per 1000 Gms.
Sat. Solution. H2O. Sat. Solution. H2O.
14.8 2. 112 2.117 45 3.648 3.661
24.6 2.612 2.619 52 4-I67 4.184
30.3 2.964 2.973 6° 4.665 4.685
36.8 3.284 3.295 70 4.213 4.231
42 3.434 3.446 80 5.185 5.212
SOLUBILITY OF MOLYBDIC ACID DIHYDRATE IN AQ. AMMONIUM SALT
SOLUTIONS. (R. and D., 1903.)
Gms. MoO3 per 1000 Gms.
t°. Solvent. . - -* -
Sat. Solution. Solvent.
29.6 10% (NH4)2SO4 18.91 19.27
31.5 io%NH4HS04 26.79 27.53
4i-8 33.22 34.36
49-7 36-32 37-69
Fusion-point data for MoO3 + Na2MoO4 are given by Groschuff (1908).
441
MORPHINE C17Hi9N03.H20.
SOLUBILITY IN SEVERAL SOLVENTS.
(U. S. P.; Muller, W., 1903.)
MORPHINE
Solvent.
Cms. Morphine per 100 Cms.
Solution.
Solvent.
Cms. Morphine per too Cms.
Solution.
At l8°-22
Water 0.0283
Alcohol
Ether 0.0131
Ether sat. with
H2O 0.0094
H2O sat. with
Ether 0.0447
Benzene 0.0625
Water 0.0254
Chloroform 0.0504
Water 0.0288
Acetone 0.128
Aq. 50 Vol. %
Acetone 0.132
Water 0.0217
Water 0.0192
°. At 25°. At 80°.
0.030 0.0961
0.600 1.31 (60°)
0.0224
(20°) (Winterstein, 1909.)
(20°)
(15°) (Guerin, 1913.)
(15°)
(15°)
(20°) (Zalai, 1910.)
(20°) (Guild, 1907.)
At i8°-22°. At 25°.
Chloroform 0.0655 0.0555
Amyl Alcohol . . . 0.8810
Ethyl Acetate 0.1861 0.1905
Petroleum
Ether 0.0854 ...
Carbon Tetra-
chloride 0.0156 0.032 (17°)
Glycerol 0.45 (15.5°)
CCL, 0.025 (20°) (Gori, 1913.)
Aniline 6.1 (20°) (Scholtz, 1912.)
Pyridine 16 (20°)
Piperidine 39.8 (20°)
Diethylamine 7.41 (20°)
50% Aq. 1 J(Baroniand
3% HaBOs J * [ 1911-)
SOLUBILITY OF MORPHINE IN SEVERAL SOLVENTS AT 25°.
Solvent.
Ethyl Alcohol
Methyl Alcohol
Chloroform
Benzene
Cms.
C17H19N03.H20
per loo cc.
Solvent.
0.388
6.66
0.04
insol.
(Schaefer, 1913.)
Cms.
Solvent.
i Vol. C2H5OH+4 Vols. CHClg
+4 Vols. C6H6
i Vol. CHsOH +4 Vols. CHCla
+4 Vols. C6H6
per 100 cc.
Solvent.
0.66
0.2
4-54
2-5
SOLUBILITY OF MORPHINE IN ETHYL ETHER AT 5.5°.
(Marcbionneschi, 1907.)
Solvent.
Washed and Distilled Ether
Ether Purified by Distillation over Na
Gms. Morphine
per 100 Gms.
Sat. Sol.
0.049
0.263
0.56
Solid
Ci7H19NO3.H2O
a
C17H19N03
SOLUBILITY OF MORPHINE IN AQUEOUS SOLUTIONS OF SALTS AND BASES AT
ROOM TEMPERATURE, SHAKEN EIGHT DAYS.
(Dieterich, 1890.)
In N/io Salt or Base. In N/i Salt or Base.
Grams per Liter. Grams rjer Liter.
[. oau or liase. /-
Salt or Base.
Morphine.
Salt or Base.
.Morphine •
NH4OH
3-51
O.2O
35-08
0-505
(NH4)2C03
4-80
0.031
48.03
0.040
KOH
4.62
2.78
46.16
. . .
K2C03
KHCO3
6.92
10.02
O.2O
O.O24
69.15
ioo. 16
0-379
0-040
NaOH
4-OO
3-33
40.05
. . .
Na2CO3
NaHC03
5-30
8.41
0.09
0.032
53-03
84.06
0.14
0.044
Ca(OH), (sat.)
i .00 (25°)
Acetate.
Hydroc
5-8l
2.4
20. Of
* 60°.
hloride.
80°.
20O.O
2.8*
Sulphate.
Apo M. Hydrochloride.
25°.
44.9
4.6
0.21
19.2
80°. '
50.0
40.0*
'25°.
6-53
0.22
80°
166.
0.
25°.
6 2.53
53* 2. 62
0.026
A" 0.053
8o°/
6.25
3-33
t.*!
>-5°'
MORPHINE 442
i
MORPHINE ACETATE CH3COOH.C17H19NO3.3H2O, Morphine
Hydrochloride HC1.C17H19NO3.3H2O, Morphine Sulphate H2SO4.
(C17H10NO3)2.5H2O, and Apo Morphine Hydrochloride HC1.C17
H17N02.
SOLUBILITY IN SEVERAL SOLVENTS.
(U. S. P.)
Grams per 100 Grams of Solvent.
Solrent.
Water
Alcohol
Chlorof
Ether
100 gms. H2O dissolve 1.69 gms. apo morphine hydrocloride at 15.5°, and 2.04
gms. at 25°.
100 gms. 90% alcohol dissolve 1.96 gms. apo morphine hydrochloride at about
15.5°. (Dott, 1906.)
100 gms. H2O dissolve 4.17 gms. morphine hydrated sulfate .5H2O at 15°.
(Power, 1882 )
MORPHINE SALTS (con.)
SOLUBILITY IN WATER AND IN 90% ALCOHOL AT ORD. TEMP.
(Squire and Caines, 1905.)
Gms. Salt per IPO cc. Gms. Salt per 100 cc.
Morphine Salt. 9o% Morphine Salt. ' 90%
H2°- Alcohol. H2°' Alcohol.
Morphine Acetate ... i Diacetyl Morphine (Heroine) o.n 2.5
" Hydrochloride ... 2 " - HC1 50 9.1
" Sulfate ... 0.143 Ethyl Morphine HCl(Dionin) 14.3 20
" Tartrate 10 0.172
100 gms. 4% HC1O4 solution dissolve 0.44 gm. morphine perchlorate at 15°.
(Hofmann, Roth, Hobald and Metzler, 1910.)
SOLUBILITY OF MORPHINE SALTS IN SEVERAL SOLVENTS AT 25°.
(Schaeffer, 1913.)
Gms. of Each Salt Separately per 100 cc. of Each Solvent.
•
Morphine Morphine Diacetyl
Hydrochloride. Sulfate. Morphine. HC HC1
95% Ethyl Alcohol 0.606 0.2 3 9.1 4
85% Ethyl Alcohol 1.2 0.4 .........
80% Ethyl Alcohol 2 0.77 .........
Methyl Alcohol ... ... 4 n.i 66. 6
Chloroform Insol. Insol. 66.6 33.3 0.526
Benzene Insol. Insol. 12.5 Insol. Insol.
i Vol. C2H5OH+4 Vols. CHC13 0.18 0.0164 66.6 4-5 5
" +4 Vols. C6H6 0.089 °-OI33 25 Q-71 I-I4
i Vol. CH3OH +4 Vols. CHC13 ... 0.22 66.6 20 20
+4 Vols. C6H6 0.253 0.066 25 6.6 8.33
Ethyl MORPHINE Ci,HHON(OH)(OC,H,). J
100 cc. H2O dissolve 0.208 gm. CnHi7OH(OH)(OC2H5) at 25°. (Schaeffer, 1912.)
" alcohol " 1.33 gms. " "
" ether " 66.6
443 Ethyl MORPHINE
Ethyl MORPHINE HYDROCHLORIDE C17H17NO(OH)(OC2H5).HC1.2H2O
(Dionin) (see also on preceding page).
SOLUBILITY IN WATER AND IN ALCOHOL. (Schaeffer, 1912.)
Cms. Ethyl Morphine HC1
per 100 cc.
t°. 'Water. Alcohol.^
IS 8-7 3-85
25 12.5 5
40 25 12. 1
50 40 20
These results differ from similar data for commercial samples of Dionin.
The differences are believed to be due to the impurities (amorphous salts of the
by-products of the ethylation) in commercial products.
100 cc. H2O dissolve 10 gms. ethyl morphine hydrochloride at ord. temp. (Dott, 19x2.)
MUSTARD OIL Allyl Isothiocyanic Ester CS:NC3H5.
SOLUBILITY IN SULFUR BY SYNTHETIC METHOD. (See Note, p. 16.)
(Alexejew, 1886.)
Gms. Mustard Oil per loo'Gms.
Sulfur Layer. Mustard Oil Layer.
90 10 72
100 12 67
tuo 15 62
120 23 51
124 (crit. temp.) 35
Freezing-point data for allyl isothiocyanate + aniline are given by Kurnakov
and Solovev (1916). Results for methyl isothiocyanate -j- phenanthrene and
methyl isothiocyanate + naphthalene are given by Kurnakov and Efrenov
(1912).
MYRISTIC ACID C13H27COOH.
SOLUBILITY IN ALCOHOLS. (Timofeiew, 1894.)
Gms. Gms.
Alcohol t° CjjH^COOH Alrnhnl t° CuH^COOH
AicohoL l ' per TOO Gms. Alcohol. t . IOQ Gms>
Sat. Sol. Sat. Sol.
Methyl Alcohol o 2.81 Propyl Alcohol o 5.6
21 21.2 " " 2i 31.2
31-5 59-2 " " 36.5 55-3
Ethyl Alcohol o 7.14 Isobutyl Alcohol o 6.4
21 31 21 28
Freezing-point data for myristic acid + palmitic acid are given by Heintz (1854).
NAPHTHALENE d0H8.
1000 cc. H2O dissolve 0.019 g™' Ci0H8 at o° and 0.030 gm. at 25°. (Hilpert, 1916.)
SOLUBILITY IN ACETIC AND OTHER ACIDS. (Timofeiew, 1894.)
Acid *• Gms. CioHg per A _: j
f0 Gms. CioHg]
i
:oo Gms. Acid,
/\C1U.
* ' 3
too Gms.'Ac
Acetic Acid
6-75
6.8
Isobutyric Acid
6.75
12.3
U (I
21-5
i3-i
Propionic Acid
6-75
13-9
{( (I
42.5
3i-i
U (t
21-5
23-4
11 t(
51-3
53-5
t( <(
50
7Q.8
(I (I
60
in
Valeric Acid
6-75
9-5
Butyric Acid
6.75
13.6
« n •
t
21-5
17.7
« «
21.5
22.1
65
167.4
« ti
60
I3I.6
NAPHTHALENE 444
SOLUBILITY OF NAPHTHALENE IN AQUEOUS AMMONIA.
(Hilpert, 1916.)
Gms. CigHg per 1000 Gms.
Solvent. Solvent at: ^
o°. 25°.
Aq. 5%NHs 0.030 0.044
Aq. 10% NHs 0.042 0.074
Aq. 25%NHa 0.064 0.162
100% NHs 33 120
Aq. 2% Pyridine 0.082 0.245
SOLUBILITY IN METHYL, ETHYL, AND PROPYL ALCOHOLS.
(Speycrs — Am. J. Sci. [4] 14, 294, '02 ; at 19.5°, de Bruyn — Z. physik. Chem. 10, 784, '92 ; at 11°, Timo
feiew — Compt. rend. 112* 11371 '91.)
The original results were calculated to a common basis, plotted on
cross-section paper, and the following table read from the curves.
In Methyl Alcohol. In Ethyl Alcohol. In F-opyl Alcohol.
t'.
Wt
Sc
. of i c<
Gms. C10H8
Wt. of i cc.
Solution.
Gms. C10H8
per 100 Gms.
C2H6OH.
Wt. of i cc.
Solution.
Gms. Cjo-^s
per loo Gms.
C3H7OH.
0
o.
8194
3
.48
O
•8175
5.0
0.8285
4-45
10
o.
812
5
.6
O
.814
7-0
0.824
5-6
20
0.807
8
.2
o
.810
9.8
0.821
8.2
25
o.
805
9
.6
o
.809
ii -3
0.820
9.6
30
o.
804
ii
.2
o
.809
13-4
O.82O
11.4
40
o.
805
16
.2
o
.812
19-5
0.823
16.4
50
0.813
26
• O
0
.822
35-o
0.837
26.0
60
o.
837
So
• O
o
•855
67.0
0.867
50.0
65
o.
870
o
.890
96.0
0.897
80.0
70
o.
9023
(68°) :
o
•930
179.0
0-933
134.1 (68
•5°)
EQUILIBRIUM IN THE SYSTEM NAPHTHALENE, ACETONE, WATER.
(Cady, 1898.)
An excess of naphthalene was added to each of a series of mixtures of water and
acetone and the temperature determined at which a second liquid phase first
appeared. Since an excess of naphthalene was present, the amount dissolved was
not known. The following supplementary experiment was, therefore, required to
ascertain the composition of the saturated solution in each case. "A weighed
quantity of naphthalene was added to a known weight of the mixed liquids, the
amount being just sufficient to cause the formation of two liquid phases. The
consolute temperature of the system was then determined and the experiment re-
peated several times with different amounts of naphthalene. If the results are
plotted, using the weights of naphthalene in a constant quantity of the mixed
liquids as abscissas and the temperatures as ordinates, we shall get a series of
curves. The composition of the liquid phase at the moment when the system
passes from solid, solution and vapor to solid, two solutions and vapor is given by
the point at which the prolongation of the curve for that particular mixture of
acetone and water, cuts the ordinate for temperature at which the change takes
place. This me^iod requires no analysis and is of advantage in this case where
ordinary quantitative analysis would be very difficult." Considerable difficulty
was experienced in determining the consolute temperatures-. It was necessary
on account of the extreme volatility of the acetone to seal the mixtures in tubes.
The table of results, calculated with the aid of the determinations made as de-
scribed above, is given on the following page.
445
NAPHTHALENE
TABLE SHOWING THE TEMPERATURES AT WHICH SOLUTIONS OF THE GIVEN COM-
POSITIONS BEGIN TO SEPARATE INTO Two LAYERS IN PRESENCE OF SOLID
NAPHTHALENE. (Cady, 1898.)
(Calculated as described on preceding page.)
Cms. per 100 Gms. Solution.
f.
65.5
53-3
45
38
32.2
28.5
28.2
The isotherms for intervals of 10° lie so close together that they are practically
indistinguishable for the greater part of their length.
SOLUBILITY OF NAPHTHALENE IN LIQUID CARBON DIOXIDE.
(Buchner, 1905-06.) (Synthetic Method used.)
Acetone.
Water.
Naphthalene.
10
89.92
0.08
ig.QI
80
0.09
29.92
69.67
0.41
4O.8l
58.22
o 97
48.67
48.68
2.65
57-43
36.64
5-93
60.43
25-75
13.82
Crit. Temp.
34-8
64
80
Gms. CnHg per
100 Gms. Sat. Sol.
8
54
IOO
loo gms. 95% formic acid dissolve 0.30 gm. naphthalene at 18.5°. (Aschan, 1913.)
100 gms. 95 % formic acid dissolve 3.44 gms. a nitronaphthalene at 18.5°. "
Data for equilibrium in the systems: naphthalene, phenol, water and naphtha-
lene, succinic acid nitrile, water, determined by the synthetic method, are given
by Timmermans (1907).
SOLUBILITY OF NAPHTHALENE IN;
Chloroform.
(Speyers; Etard.)
Carbon Tetra Carbon Di
Chloride, Sulphide.
(Schroder — Z. physik. (Arctowski — Compt
Ch. ii, 457/93.) rend. 121, 123/95; Etard.)
ft0 Wt. of i cc.
Solution.
Gms. C10H8 per
100 Grama
CHCJa.
Gms. CioH8 per
too Gms. SaL
Solution,
Oms. C-iQrig per
too Gms. Sat.
Solution.
-108
•
...
0.63
-82
. 1 .
1.38
~~~ 5°
23
-30
8.8
6.6
— 10
15-6
...
14.1
0
•393
19-5
9-0
19.9
+ 10
•355
25-5
I4-O
27-5
20
.300
31.8
20-0
36-3
25
.280
35-5
23-0
41 -o
30
•255
40.1
26.5
46.0
40
.205
49-5
35-5
57 -2
50
.150
60.3
47-5
67.6
60
.090
62.5
79-2
70
.040
87^2
80.0
9° -3
NOTE. — Speyers' results upon the solubility of C10H8 in CHC13,
when calculated to grams per 100 grams of solvent, agree quite well
with Etard's (Ann. chim. phys. [712 570, '94 figures, reported on the
basis of grams C10H8 per 100 grams saturated solution.
NAPHTHALENE
446
Benzene.
SOLUBILITY OF NAPHTHALENE IN:
(Schroder; Etard; Speyers.)
Chlor Benzene. Hexane.
50
20
O
10
20
25
30
40
50
60
70
80
Gms. CioH8
per 100 Gms.
Solution.
27
36
40
45
54
65
77
88.0
Gms. CioHg
per 100 Gms.
Solution.
24.0
31.0
39-o
48.0
57-5
70-5
85.0
Gms. C10H8
per loo Gms.
Solution.
o-3
1.9
5-5
9.0
14.0
17-5
21 .0
30.8
43-7
60.6
78.8
Toluene.
wt. of i cc.
Solution.
0.9124
0.9126
0-9I35
0-9I55
0.9180
0.9250
0.9350
0-9475
o . 9640
0.9770
Gms. CioH8
per 100 Gms.
C6H5.CH3.
15-0
28.0
36.0
42.O
56.0
69-5
83.0
97-5
III.O
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
naphthalene and each of the following compounds:
ttNaphthol. (Crompton & Whitely, 1895; Kuster,
'95; Vignon, '91 ; Miers & Isaac, 'o8a.)
ft Naphthol. (Crompton & Whitely, 1895; Vignon,
iSgirlsaac, 1908.)
a Naphthylamine. (Vignon, 1891.)
0
Dihydronaphthalene. (Kuster, 1891.)
Nitronaphthalene. (Palazzo & Battelli, 1883.)
Palmitic Acetic Ester. (Batelli & Martinetti, '85.)
Paraffin. (Palazzo & Battelli, 1883.)
Phenanthrene. (Vignon, 1891; Miolati, 1897.)
Phenol. (Yamamoto, '08; Hatcher & Skirrow, '17.)
0 Nitrophenol. (Saposchinikow, '04 ; Kremann, '04.)
p Nitrophenol. (Kremann, 1904.)
2.4 Dinitrophenol. ( (Saposchinikow, 1904;
Picric Acid. ( Kremann, 1904.)
Pyridine. (Hatcher & Skirrow, 1917.)
Pyrocatechol. (Kremann & Janetzky, 1912.)
Resorcinol. (Vignon, 1891; Kremann &
Janetzky, 1912.)
Stearic Acid. (Gourtonne, 1882.)
Sulfur. (Bylert, .)
Nitrotoluene. (Kremann, 1904.)
i.2.4Dinitrotoluene. "
1 .2 .6 " (Kremann & Rodinis, 1906.)
1.34
I.3;5
Trinitrotoluene. (Kremann, 1904.)
P Toluidine. (Vignon, 1891.)
Thymol. (Roloff, 1895.)
F.-pt. data are also given for the following mixtures:
Nitronaphthalene + Paraffin. (Campetti & Delgrosso, 1913; Palazzo & Batelli, 1883.)
a Nitronaphthalene + Urethan. (Mascarelli, 1908.)
a Nitronaphthalene + « Naphthylamine. (Tsakalotos, 1912.)
NAPHTHALENE SULFONIC ACID C10H7SO3H.
SOLUBILITY IN AQUEOUS HYDROCHLORIC ACID AT 30°.
(Masson, 1912.)
dyoi Sat.
Solution.
.1925
•1653
•1553
.1115
.1197
.1569
Mols. per Liter Sat. Sol.
HC1.
C10H7SO,H.
0
3 • 263
I.29I
2.470
1.826
2.117
4.017
0.762
7.232
0.089
0.88
0.063
Gms. per Liter Sat. Sol.
HC1.
C10H7S03H.
O
679
47.08
5H
66.59
440.6
146.5
158.6
263.7
I8.5
300.3
I3-I
447 NAPHTHOIC ACID
0 NAPHTHOIC ACID Ci0H7COOH.
One liter of aqueous solution contains 0.058 gm. Ci0H7COOH at 25°.
(Paul, 1894.)
Dihydro p NAPHTHOIC ACIDS Ci0H9COOH (118° and 161° isomers).
SOLUBILITY OF EACH ISOMER, DETERMINED SEPARATELY, IN WATER.
(Derick and Kamra, 1916.)
cc. o.oi n Ba(OH)2 Solution Required
AO per 10 cc. of the Sat. Solution of the:
118° Isomer.
161° Isomer.
0
0-39
O.I9
20
0.56
o-34
40
1-34
0.69
55-56
2.89
i-45
71-72
6.7
3.48
80
9-3
4.68
00
14.6
8
96-97
20.1
io-5
P NAPHTHOL CioHyOH.
SOLUBILITY IN WATER.
Gms.0C10H7OH
t°. per 100 cc. Authority.
Sat. Sol.
12.5 0 . 044 (Kuriloff, 1897.)
25.1 0 . 074 (Kttster, 1895.)
29.5 0.0876 (Kuriloff, 1898.)
Data for the solubility of isomorphous mixtures of 0 naphthol and naphthalene
in water at 25.1° are given by Kiister (1895).
SOLUBILITY OF /3 NAPHTHOL IN AQUEOUS SOLUTIONS OF PICRIC ACID AT 29°.
(Kuriloff, 1898.)
Mols. X lo6 per 100 cc. Solution. Gms. per 100 cc. Solution.
QH2.OH(N02)3.
C,0H7OH.
C6H2OH(N02)3.
Ci0H7OH.
Solid Phase.
0
609
O
0.0877
0 Naphthol
54
615
0.0124
0.0886
"
68.5
62O
0.0157
o . 0894
" +/3 Naphtholpicrate
69
607
0.0158
0.0875
0 Naphtholpicrate
69
597
0.0158
0.0860
•
88
494
O.O2I2
O.O7I2
•
100
390
0.0229
0.0562
"
196
180
O.O449
0.0259
«
308
105
o . 0706
O.OI5I
«
933
8
0.2138
O.OOII
" +PicricAcid
928
0
O.2I26
0
Picric Acid
Data are also given for the distribution of 0 naphthol between water and ben-
zene. The mean of the cone, in C6H6 layer divided by cone, in H2O layer is given
as 67. The temperature is not given. The determination of the ft naphthol was
made by an iodine titration method.
The coefficient of distribution of /3 naphthol between H2O and CHClj at 25° is;
cone, in H2O -5- cone, in CHCls = 0.0171. (Marden, 1914.)
Data for the solubility of /9 naphthol, picric acid (naphthol picrate) and their
mixtures in benzene, determined by the synthetic (sealed tube) method, are given
by Kuriloff (i897a).
100 cc. 90% alcohol dissolve about 55 gms. /3 Ci0H7OH at 15.5°.
(Greenish and Smith, 1903.)
100 gms. 95% formic acid dissolve 3.11 gms. /3 C10H7OH at 18.6°. (Aschan, 1913.)
NAPHTHOL 448
SOLIDIFICATION TEMPERATURES OF MIXTURES OF ft NAPHTHOL AND SALOL.
(Bellucci, 1912.)
t° of Cms. 0 CioH7pH per t° of Cms. 0 C10H7OH per
Solidification. 100 Cms. Mixture. Solidification. 100 Gms. Mixture.
121.7 ioo 80 40
116.5 9° 68 30
in 80 52.5 20
105 70 34 Eutec. 10
97-5 °° 38.5 5
88 - - 50 42 o
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES:
a Naphthol + a. Naphthylamine. (Vignon, 1891.) ^
+ ft
+ Dimethylpyrone. (Kendall, 1914.)
-j- Resorcinpl. (Vignon, 1891.)
+ p Toluidine. (Vignon, 1891; Philip, 1903.)
ft Naphthol + a Naphthol. (Vignon, 1891; Crompton and Whiteley, 1895.)
" + a Naphthylamine (Vignon, 1891.)
+ /3.
+ Dimethylpyrone (Kendall, 1914.)
+ Picric Acid. (Kendall, 1916.)
-j- Sulfonal (Bianchini, 1914.)
+ p Toluidine. (Vignon, 1891.)
a NAPHTHYLAMINE p Sulfonic Acid, 1.4 a. Ci0H6NH2.SO3H.
a NAPHTHYLAMINE o Sulfonic Acid, 1.2 a doHeNHi.SOsH.
SOLUBILITY OF EACH SEPARATELY IN WATER.
(Dolinski, 190? "*
Gms. per ioo Gms.H2O. Gms. per ioo Gms. H2O.
t°.
p Sulphonic
o Sulphonic
t°.
p Sulphonic
o Sulphonic
Ac.
Ac.
Ac.
Ac.
0
0.027
0.24
50
0.059
0.81
10
O.O29
0.32
60
0-075
I .01
20
0.031
0.41
70
0.097
i .37
30
0.037
0.52
80
0.130
1. 80
40
0-048
0.65
90
0.175
2 .40
IOO
0.228
3-19
The coefficient of distribution of ft naphthylamine between benzene and watei
at 25° is; cone, in C6H6-:- cone, in H2O = 279. The coefficient for a naphthyla
mine, similarly determined, is 252. (Farmer and Warth, 1904 )
FREEZING-POINT DATA ARE GIVEN FOR THE FOLLOWING MIXTURES:
a Naphthylamine + Phenol. (Philip, 1903.)
+ Quinol. (Philip & Smith, 1905.)
+ Resorcinpl. ( " ; Vignon, 1891.)
+ p Toluidine. (Vignon, 1891.)
ft Naphthylamine -j- Phenol. (Kremann, 1906.)
-j- Rescorcinol. (Vignon, 1891.)
+ p Toluidine.
P NAPHTHYL BENZOATE C6H5COOC10H7.
ioo gms. 95% formic acid dissolve 0.25 gm. CeHsCOOCioHr at 18.6°.
(Aschan, 1913.)
NARCEINE C23H27N08 + 3H2O.
ioo gms. H2O dissolve 0.076 gm.'narceine at 13°; ioo gms. 80% alcohol dissolve
0.105 gm. at 13°.
ioo gms. CC14 dissolve o.on gm. narceine at 17° (Schindelmeiser, 1901); 0.002
gm. at 20° (Gori, 1913).
449
NARCOTINE
NARCOTINE C20H23NO7.
SOLUBILITY
IN
SEVERAL SOLVENTS.
Solvent.
t°.
Gms. Narcotine per
100 Gms. Solvent.
Authority.
Water
15
0 I*
(Guerin, 1913.)
Water
20
O.OO445
(Zalai, 1910.)
Acetone
15
41.96*
(Guerin, 1913.)
Aq. 50 Vol. % Acetone
15
0.7*
«
Aniline
20
25
(Scholtz, 1912.)
Pyridine
2O
2-3
«
Piperidine
20
«
Diethylamine
2O
0.4
«
Carbon Tetrachloride
2O
1.04
(Gori, 1913-)
Trichlor Ethylene
15
6.5
(Wester and Bruins, 1914.)
Oil of Sesame
2O
0.086
(Zalai, 1910.)
* Per 100 cc. solvent.
NEODYMIUM CHLORIDE NdC1.6H2O.
SOLUBILITY IN WATER. (Matignon, 1906, 1909.)
Method of obtaining saturation not stated.
Cms. NdCl3 per 100 Cms. Cms. NdCl3.6HoO per 100 Gms.
jj
Sat. Sol.
1.74
Sat. Sol. Water. Sat. Sol. Water.
13 1-74 49-67 98.68 71.12 246.2
100 ... ... 140
100 gms. abs. alcohol dissolve 44.5 gms. (anhydrous) NdCl3 at 20°. Saturation
was obtained by spontaneous evaporation of the solution over H2SO4.
(Matignon, 1906.)
100 gms. anhydrous pyridine dissolve 1.8 gms. anhydrous NdCl3 at about 15°.
Saturation obtained by daily agitation of the solution for some weeks. (Matignon, '06.)
NEODYMIUM COBALTICYANIDE Nd2(CoC6N6)2.9H2O.
looogms.aq. io%HCl (di5 = 1.05) dissolve 4. 19 gms. salt at 25°. (James & Willand, '16.)
NEODYMIUM GLYCOLATE Nd(C2H3O3)3.
One liter H2O dissolves 4.609 gms. salt at 2O°. (Jantsch & Grimkraut, 1912-13.)
NEODYMIUM MOLYBDATE Nd2(MoO4)3.
One liter H2O dissolves 0.0186 gm. salt at 28° and 0.0308 gm. at 75°. The
mixtures were frequently stirred at constant temperature during only two hours.
(Hitchcock, 1895.)
NEODYMIUM Double NITRATES.
SOLUBILITY IN AQ. HNO3 OF d^= i.325( = 51.59 GMS. HNO3 PER
100 CC.) AT 16°. (Jantsch, 1912.)
Gms. Hydrated
Double Salt. Formula. Double Salt per
100 Gms. Sat. Sol
Neodymium Magnesium Nitrate [Nd(NO3)6]2Mg3.24H2O 97.7
Nickel " " Ni3 " 116.6
Cobalt " " CO3 " 151.6
Zinc " " Zn3 " 177
Manganese " Mn3 " 296
NEODYMIUM OXALATE Nd2(C2O4)3.ioH2O.
SOLUBILITY IN WATER AT 25° BY ELECTROLYTIC DETERMINATION.
(Rimbach and Schubert, 1909.)
One liter sat. solution contains 0.0053 mg- equivalents of anhydrous salt = 0.49
milligram.
SOIJUBILITY IN AQUEOUS 20% SOLUTIONS OF METHYL, ETHYL AND TRIETHYL
AMINE OXALATBS, ROUGHLY DETERMINED. (Grant and James, 1917.)
100 cc. aq. 20% methyl amine oxalate dissolve 0.027 gm. neodymhim oxalate.
" ethyl " " " ai07 "
" triethyl " ^ " 0.065 "- "
NEODYMIUM OXALATE 450
SOLUBILITY OF NEODYMIUM OXALATE IN AQUEOUS SOLUTIONS OF
NEODYMIUM NITRATE AT 25°. (James and Robinson, 1913.)
(The mixtures were constantly agitated at constant temperature for twelve
weeks.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
Solid Phase.
Nd2(C204)3.
Nd2(NO3)6.
Nd2(C204)3.
Nd2(N03)6.
0.18
6.46 Nd2(C204)3.nH20
2.07
47.64
0-54
12.23
2-54
50-52
0.76
17.78
2.89
52.82
0.85
22.67
3-17
54.67
0.96
27-43
2.21
56.48Pr.
1.28
3I-36 "
1.44
59.68
1.38
1.33
59-67
1.66
38^0
I. 21
59-70
1.88
42.13
0.96
59-75
1.96
44.82
60.46
1.2^.24
Nd2(NO3)6(?H20)
4)3.2|Nd2(N03)6.24H20.
NEODYMIUM Dimethyl PHOSPHATE Nd2[(CH3)2PO4]6.
100 gms. H2O dissolve 56.1 gms. Nd2[(CH3)2PO4]6 at 25° and about 22.3 gms.
at 95°- (Morgan and James, 1914.)
NEODYMIUM SULFATE Nd2(SO4)3.
SOLUBILITY IN WATER.
(Muthmann and Rolig, 1898.)
Gms. Nd2(SO4)^ per 100 Gms. Gms. Nd2(SO4)3 per TOO Gms.
Solution. Water. Solution. Water.
o 8.7 9.5 50 3.5 3.7
16 6.6 7.1 80 2.6 2.7
30 4.7 5 108 2.2 2.3
NEODYMIUM SULFONATES.
SOLUBILITY IN WATER.
Gms. Anhy-
Sulfonate. Formula. t°. dr™Qs Q^f61 Authority.
H2O.
Neodymium :
m (Nitrobenzene Nd[C6H4(NO2)SO3]3.6H2O 15 46.1 (Holmberg, 1907.)
Bromo} Sulfonate Nd[C6H3Br(i)NO2(4)SO3(3)]3.8H2O 25 7.25 (Katz& James, 1913.)
NEODYMIUM TUNGSTATE Nd2(WO4)3.
One liter H2O dissolves 0.0190 gm. Nd2(WO4)3 at 22°, 0.0168 gm. at 65° and
0.0152 gm. at 98°. The mixtures were not constantly agitated and only two
hours were altowed for saturation. (Hitchcock, 1895.)
NEON Ne.
SOLUBILITY IN WATER.
(v. Antropoff, 1909-10.)
t°. o. 10. 20. 30. 40. 50.
Coef. of Absorption /? 0.0114 0.0118 0.0147 0.0158 0.0203 0.0317
The results are in terms of the coefficient of absorption as defined by Bunsen
(see p. 227) and modified by Kuenen, in respect to substitution of mass of H2O
for volume of H2O in the formula Absorp. coef. Kuenen = — ~rrrv> vx r>*
mass of H2O X P
NEURINE PERCHLORATE CH2.CH.N(CH3)3ORHC1O4.
100 gms. EUO dissolve 4.89 gms. of the salt at 14.5° (Hofmann & Hobold, 1977.)
451
NICKEL BROMATE Ni(BrO3)2.6H2O.
100 gms. cold water dissolve 27.6 gms. nickel bromate.
NICKEL BROMATE
NICKEL BROMIDE
NiBr2.6H2O.
SOLUBILITY IN WATER.
(Etard, 1894.)
t°.
-20
— io
o
+ 10
20
Gms. NiBrt
per 100 Gms.
Solution.
47.
50.
53
55
56.
t°.
25
30
40
50
60
Gms. NiBr,
per 100 Gms.
Solution.
57.3
58
59.1
60
60.
t°.
80
ioo
120
140
NICKEL CARBONATE NiCO3.
One liter H2O dissolves 7.?8<)\X io~* mols. NiCO3
NICKEL CARBOXYL.
Gms. NiBrj
per 100 Gms.
Solution.
60.6
60.8
60.9
6 1
0.0925 gm. at 25°.
(Ageno and V
(Ageno and Valla, 1911.)
ioo gms. of the aqueous solution saturated at 9.8° contain 2.36 cc. of the vapor
6.43 milligrams Ni. In blood serum it is 2 \ times as soluble. (Armit, 1907.)
NICKEL CHLORATE Ni(ClO3)2.
SOLUBILITY IN WATER.
(Meusser — Ber. 35, 1419, '02.)
48
55
65
79-5
-13-5
— 9 26.62
Sp. Gr. of solution saturated at + 18 = 1.661.
According to Carlson (1910) ioo gms. sat. sol. in H2O at 16° contain 64.1 gms.
Ni(ClO3)2 and du of sat. sol. = 1.76.
Gms.
Mols.
t°
Ni(ClO3)2
Ni(C103)2
Solid
per ioo Gms,
Solution.
. per ioo
Mols.H2O
Phase.
-18
49-55
7.84
Ni(ClO3)2.6H2O
- 8
5J-52
8.49
"
o
52.66
8.88
"
+ 18
56-74
10-47
"
40
64.47
15.35
it
Gms. Mols.
Ni(ClO3)2 Ni(ClO3)2
per ioo Gms. per ioo
Solid
Phase.
Solution. Mols. H2O.
67.60 16.65
Ni(C103)24H,0
68.78 17.59
•4
69.05 iS.OI
«
75.50 24.68
•
3J-85 3-73
Ice
2.90
NICKEL PerCHLORATE Ni(ClO4)2.9H2O.
SOLUBILITY IN WATER.
(Goldblum and Terlikowski, 1912.)
Gms
O
10.9
21.3
30.7
49
30.7
H20.
O
33.19
46.68
70
..
90
Ice
Ice + Ni(ClO4)3.9H2O
—21.3
9
7-5
18
26
45
Gms.
H20.
.. 92.5["Ni(ClO4)s9H»0
573 104.6 Ni(ClO4),.sH,Q
576 1 06. 8 Ni(C10<)3.sH,0
576 no.i
584 112. 2
594 1 18. 6
NICKEL CHLORIDE
452
NICKEL CHLORIDE NiCl2.6H2O.
SOLUBILITY IN WATER.
(Etard, 1894.)
t-.
Gms. NiCU
per ioo Gms.
Solution.
«-.
Gms. NiClj
per ioo Gms.
Solution.
t°.
Gms. NiCl2
per ioo Gms.
Solution.
-17
29.7
25
40
60
45.1
o
35
30
40.8
70
46
+ 10
37-3
40
42.3
78
46.6
20
39 -1
50
43-9
IOO
46.7
1000 cc. sat. HC1 solution dissolve 4 gms. NiCl2 at 12°. (Ditte, 1881.)
100 gms. abs. alcohol dissolve 10.05 Sms- NiCl2 at room temperature.
100 gms. abs. alcohol dissolve 53.71 gms. NiCl2.6H2O at room temperature.
(Bodtker, 1897.)
100 gms. abs. alcohol dissolve 2.16 gms. NiCl2.7H2O at 17°, and 1.4 gms. at 3°.
(de Bruyn, 1892.)
100 gms. saturated solution in-glycol contain 16.2 gms. NiCl2 at room tem-
perature, (de Coninck, 1905.)
loo cc. anhydrous hydrazine dissolve 8 gms. NiCl2 at room temp, and solu-
tion is colored violet. (Welsh and Broderson, 1915.)
ioo gms. 95% formic acid dissolve 5.9 gms. NiCl2 at 20.5°. (Aschan, 1913.)
When i gm. of nickel, as chloride, is dissolved in ioo cc. of 10% aq. HC1 and
shaken with ioo cc. of ether, o.oi per cent of the Nickel enters the ethereal layer.
(Mylius, 1911.)
NICKEL CITRATE Ni3[(COOCH2)2C(OH)COO]2.2H2O.
'ioo cc. sat. solution in water contain 0.28 gm. Ni =[0.94 gm. anhydrous
salt at IO°. (Pickering, 1915.)
NICKEL Potassium CITRATE K4Ni[(COOCH2)2COHCOO]2.
ioo cc. sat. sol. in water contain 3.9 gms. Ni = 41 gms. salt at 10°.
(Pickering, 1915.)
NICKEL HYDROXIDE Ni(OH)2.
Aqueous ammonia solutions of nickel hydroxide were evaporated in a vacuum
desiccator and samples withdrawn at intervals for analysis. The results obtained
in duplicate series yielded different curves. For 2 n NHs the gms. Ni per liter
varied from 0.17 to 0.83. For 4 n NH3, the gms. Ni per liter varied from 0.36
to 1.8. (Bonsdorff, 1904.)
NICKEL IODATE Ni(IO3)24
SOLUBILITY IN WATER.
(Meusser — Ber. 34, 2440, *oi.)
Gms. Mols. Gms. Mols.
to Ni(IO3)2 Ni(IO3)2 Solid to Ni(IO3)2 Ni(IO3)2 Solid
' per ioo Gms. per ioo Mols. Phase. ' per ioo Gms. per ioo Mols. Phase.
Solution. H2O. Solution. H2O.
0 0-73 0.033 Ni(I03)24H20 18 0.55 0.0245 Ni(IOa)2.2H20 (a)
18
I -01
0.045
50 0.81
0-035
1C
30
1.41
0.063
75
•03
0.045
tc
O
o-53
0.023
Ni(I03)2.2H20 (i) 80
.12
O.O49
It
18
0.68
0.030
30
•135
O.05O
Ni(I03)2
30
0.86
0.039
.07
0-046
"
50
1.78
0.080
75
.02
0.045
"
8
0.52
0.023
Ni(I03)2.2H2O (2) 90 0.988
0.044
M
(i) a Dihydrate.
(2) /3 Dihydrate.
453
NICKEL IODIDE
NICKEL IODIDE NiI2.6H2O.
— 20
O
IO
20
Gms. NiI2 per
100 Gms. Solution
52
55-4
57-5
59-7
IN WATER. (Etard, 1894.)
xo Gms. Nil2 per
loo Gms. Solution.
to Gms. NiI2 per
100 Gms. Solution.
25
60.7
60
64.8
30
61.7
70
65
40
63.5
80
65.2
50
64.7
90
65-3
By interpolation the tr. pt. for NiI2.6H2O + NiI2.4H2O is at 43°.
NICKEL MALATE Ni[CH2CHOH(COO)]2.3H2O.
loo cc. sat. solution in water contain 0.02 gm. Ni = 0.06 gm. salt_at ip°.
NICKEL NITRATE Ni(NO3)2.
SOLUBILITY IN WATER.
(Funk — Wiss. Abh. p. t. Reichanstalt, 3, 439, *oo.)
(Pickering, 1915.)
Gms. Mols.
Ni(NO3)2 Ni(N03)2 Solid
per 100 Gms. per 100 Mols. Phase.
Solution. H2O.
Ni(NO3)2.9H2O
Ni(N03)2.6H20
-23
39
.02
6-31
— 21
39
.48
6-43
— 10
•5 44
•13
7-79
— 21
39
•94
6-55
— 12
•5 4i
•59
7.01
— 10
42
.11
7.16
- 6
43
.00
7-44
O
44
•32
7.86
+ 18
48
•59
9-3
Gms. Mols.
Ni(N03)2 Ni(NO3)2 SoUd
per 100 Gms. per 100 Mols. Phase.
Ni(NOa)2.6H2O
Ni(N03)3.3H20
Solution.
H2O.
20
49.06
9-49
41
55-22
12. 1
S^
•7 62.76
I6.7
58
61.61
J5-9
60
61.99
16.0
64
62.76
16.6
70
63-95
17.6
90
70.16
23.1
95
77.12
33-3
100 gms. sat. solution in glycol contain 7.5 gms. Ni(NO3)2 at room temperature.
(de Coninck.)
100 cc. anhydrous hydrazine dissolve 3 gms. Ni(NO3)2 at room temp.
(Welsh and Broderson, 1915.)
NICKEL OXALATE Ni(COO)2.
100 gms. 95% formic acid dissolve o.oi gm. at 19.8°. (Aschan, 1913.)
NICKEL SULFATE NiSO4.7H2O.
SOLUBILITY IN WATER. (Steele and Johnson, 1904; see also Tobler, Etard and Mulder.)
Grams NiSO4 per
*o zoo Gms. Solld
* • * T>U«««
t°
Grams NiSO4 per
100 Gms.
Solid
Phase.
Solution.
Water.'
Solution.
Water.
-5
20
•47
25
. 74 NiSO4.7H2O
33
• O
30
•25
43
•35
NiSO4.6H2O
0
21
.40
27
.22
35
.6
30
•45
43
•79
• (blue)
9
23
•99
31
•55
44
•7
32
•45
48
•05
"
22 .6
27
.48
37
.90
5°
.0
33
•39
5°
.15
"
30
29
•99
42
.46
53
.0
34
•38
52
•34
"
32-3
30
•57
44
• O2 "
54
•5
34
•43
52
•50
NiSO4.6H2O
33
31
•38
45
•74
57
.0
34
.81
53
.40
" (green)
34
31
.20
45
•5
60
35
•43
54
.80
"
32-3
30.35
43
.57 NiSO4.6H2O
7°
37
•29
59
•44
"
33 -°
30
•25
43
•35 " <blue>
80
38
.71
63
•17
M
34-o
30
•49
43
•83
99
43
.42
76
•71
M
Transition points, hepta hydrate <=± hexa hydrate = 31.5*
Hexa hydrate (blue) ^± hexa hydrate (green) = 53.3°.
NICKEL SULFATE
454
SOLUBILITY OF MIXTURES OF NICKEL SULPHATE AND COPPER SULPHATE.
Results
at 35°.
Gms. per 100 Gms. H^.
Mol. per cent in Solution.
Mol. per cent in Solid Phase. Crystal
CuSO4.
NiSO4. *
CuS04.
NiSO4/
'CuS04.
NiSO4.
Form.
9.62
583-9
1.57
98.43
o-35
99-65
Rhombic
41.66
484.4
7.69
92.31
2.12
97.88
"
75-39
553-5
11.66
88.34
4.77
95-23
Tetragonal
106.40
506-5
16.92
83.08
6-52
93-48
"
172.0
483.8
25-63
74-37
13.88
86.17
"
186.9
468.0
27.90
72.IO
(I8.77
(94.91
81-23
5-09
Tetragonal
Triclinic
Results
at 67°.
20.04
729-3
2.65
97-35
o-93
99.07
Monociinic
66.01
706.2
8.3I
91.69
2.86
97.14
"
88.08
501.6
86.45
3-92
96.08
•«
47-94
675.0
16.39
83.61
6.66
93-34
»
249-9
747-8
24.46
75-54
22.32
77.68
f Monociinic
I Triclinic
SOLUBILITY OF MIXTURES OF NICKEL SULPHATE AND SODIUM SUL-
PHATE, ETC.
(Koppel; Wetzel — Z. physik. Chem. 52, 401, '05.)
Gms. per 100
t°. Gms. Solution.
Gms. per 100
Gms.H2O.
Mols. per 100
Mols. H2O.
SoKd
Dl
NiS04.
Na8S04.
NiS04.
Na2S04.
'NiS04. Na2S04. ' fudx'
O
16
•94
7
.61
22
.46
10
.09
2
.61 1.28 "
.
5
17
•99
IO
•85
25.28
J5
.24
2
•94 1-93
NiS04.7H20 +
Na2SO4.ioH2O
10
18
•97
I3-85
28
.26
20
.64
3
.29 2.61
20
18
.76
17
.21
29
•3i
26
.87
3
.410 3.404
NiNa2(S04)24HaO
25
17
•85
16
•54
27
•33
25
•33
3
.181 3.208
«
30
16
•74
15
•34
24
.64
22
•58
2
.868 2.861
it
35
16
.28
14
.91
23
.66
21
.67
2
•753 2.744
-
40
15
•35
14.49
21
.88
20
•65
2
.546 2.616
i*
18.5
'9
.61
16
•49
30
.70
25
.80
3
•S6 3-27 *
20
20
•i3
16
•IS
•59
25
•35
3
.67 3.21
25
21
.20
14
•77
33
.11
23
.06
3
.85 2.92
f NiNa2(SO4)2.4H2O H-
30
22
.60
12
.80
34
.98
19
.82
4
.07 2.59
NiSO4.7H2O
35
23
.62
10
.78
36
.01
16
•43
4
.19 2.08
40
24
.92
9
•39
37
•93
14
.29
4
.41 1.81 -
18.5
16
.80
18
•93
26
.14
29
•45
3
.04 3-72 "
20
15
.48
20
.18
24
.06
31
•37
2
.80 3.97
25
10
.92
24
.12
16
.81
37
•13
I
.96 4.70
a
30
6.40
28
•71
9
.87
I
.15 5.60 -
35
4
•54
3i
•65
7
•13
49
•59
O
.838 6.28
NiNa2(S04)2.4H20 +
40
4
•63
3i
•37
7
.24
49
•03
o
.843 6.21
j Na2S04
455 NICKEL SULFATE
SOLUBILITY OF NICKEL POTASSIUM SULFATE NiK2(SO4)2.6H2O IN WATER.
(Tobler, 1855; v. Hauer, 1858.)
Cms. NiK2(SO4)2 per 100 Gms. H2O. o Cms. NiK^SOQa Per 100 Cms. H2O.
(Tobler.) (v. Hauer.) (Tobler.) (v. Hauer.)
o 5.3 ... 50 30
10 . 8.9 ... 60 35.4 20.47
20 13.8 9.53 70 42
30 18.6 ... 80 46 28.2
40 24 14.03
SOLUBILITY OF NICKEL SULFATE IN AQUEOUS SOLUTIONS OF METHYL
ALCOHOL AT 14°.
(de Bruyn, 1903.)
Small test tubes of 4-6 cc. capacity'were used. They were almost completely
filled with the salt and solvent and placed in the bath in an inclined position
with salt occupying the upper part of the tube. This caused a "spontaneous
circulation of the solvent." The solutions were analyzed by precipitating NiO
with KOH at the boiling point, in porcelain vessels.
Wt. Per cent
VJII
is. rNio»~»4 per 100 vjiii
s. oai. oui. 111 \_uuuitt \
mtun
CH3OH
in Solvent.
NiSO4.7H2O as
Solid Phase.
NiSO4.6H2O a as
Solid Phase.
NiSO4.6H2O /3 as
Solid Phase.
NiSO4.4H2O as
Solid Phase.
o (H20)
26.4
26 (low)
27.2
25.1
10
19.7
22(?)
20-4
20
14.7
14
14.8
30
6^8
6.6
7-5
. . .
40
2.8
2.4
3.1
50
1.3
i
1.4
1.4
60
0.8
0.4
0.6
70
0.6
0.2
0.4
80
0.65
0.2
0.4
0.66
85
*-5
°-3
0.7
90
5-7
1.2
2-5
95
ii
6
9 (?)
. . .
100
16.8
12.4 (low)
15.7 (low)
7-38
NiSO4.6H2O a is greenish blue. NiSO4.6H2O is more greenish than the a salt.
SOLUBILITY OF NiSO4.3CH3OH.3H2O IN 'AQUEOUS CH8OH AT 14°.
(de Bruyn, 1903-)
Wt. Per cent
CH3OH.
Gms. NiSO4 per
100 Gms. Sat. Sol.
Wt. Per cent
CH3OH.
Gms. NiSO4 per
100 Gms. Sat. Sol.
85
I .93
90
0.70
86
I .73
92-5
0.50
87
1.48
95
0-455
88
1-25
97-5
0-77
89
1. 01
100
3-72
Approximately two hours were allowed for attainment of equilibrium.
In solutions containing more than 15% H2O the salt is gradually transformed
toNiSO4.6H2O0.
100 gms. absolute ethyl alcohol dissolve 1.4 gm. NiSO4-7H2O at 4° and 2.2
gms. at 17°. (de Bruyn, 1892.)
100 gms. sat. solution in glycol contain 9.7 gms. NiSO4 at room temp.
(de Coninck, 1905.)
NICKEL SULFIDE NiS.
One liter H2O dissolves 39.9 X lO"6 gm. mols. NiS = 0.0036 gm. at 18°, by
conductivity method. (Weigel, 1906.)
Fusion-point data for Ni2S-fNa2S and Ni3S2+Na2S are given by Friedrich (1914).
NICOTINE
NICOTINE Ci0Hi4N2.
456
SOLUBILITY IN WATER.
(Hudson, 1904.)
Determinations made by Synthetic Method, for which see Note, page 16.
Below 60° and above 210° both liquids are miscible in all proportions; likewise
with percentages of nicotine less than 6.8 and above 82 per cent the liquid does
not show two layers at any temperature. Below 94° the upper layer is water.
Above 94° the upper layer is nicotine. The curve plotted from the following
results makes a complete circle.
Percentage of
Nicotine
in the Mixture.
6.8
7.8
10.0
14.8
32.2
49.0
66.8
80.2
82.0
Temperature of
Appearance of
Temperature of
94
89
75
64
72
87
129
95
155
200
210
205
190
170
I30
Additional data for the above system are given by Tsakalotos (1909). The
values for the temperatures of saturation are in general, from i° to 5° lower than
those of Hudson.
NIOBIUM Potassium FLUORIDE NbK2F7.
SOLUBILITY IN WATER AND IN AQUEOUS HF AND AQUEOUS KF SOLUTIONS.
(Ruff and Schiller, 1911.)
' The determinations were made in platinum vessels. The mixtures were
shaken for 3 hour periods at constant temperature and the saturated solutions
filtered through platinum funnels.
Gms. per 100 Cms. Sat. Solution.
NbF6.
KF.
HF.
ooiiu .ruase.
Water
16
5-IQ
2.98
o-35
K2NbOF6.H2O
a
16
7.07
5-33
4-35
K2NbOF5.H2O+K2NbF7
Aq. 10.95% HF
16
4-33
2.32
10.43
K2NbF7
" 7-4i%KF
16
1.16
5-54
0.13
K2NbOF5.H2O
" 7-39% EF
16
2.67
6.04
5-39
K2NbOFs.H2O+K2NbF7
Water
85
30-39
14.68
0-35
K2NbOFs.H20(?)
Aq. 4.8i%KF
80
11.66
10. 08
i-53
"
NITRIC ACID HNO3.
DISTRIBUTION OF NITRIC ACID BETWEEN WATER AND ETHER AT 25°.,
(Bogdan, 1905, 1906.)
Mols. HNO3 per Liter of: Mols. HNO, per Liter of:
H2O Layer.
0.9145
0.4811
o . 2644
0.1392
Ether Layer.
0.0855
0.0278
o . 00894
O.OO278
H2O Layer.
0.09005
0.04749
0.02760
0.02462
Ether Layer.
O.OOlSl
0.00064
0.00029
0.00025
457
NITRIC ACID
RECIPROCAL SOLUBILITY OF NITRIC ACID AND WATER, DETERMINED BY THE
FREEZING-POINT METHOD.
(Kiister and Kremann, 1904; see also Pickering, 1893.)
Gms. HN03
t°. per^ioopms. Solid Phase. t°.
Gms. HNO3
per 100 Gms. Solid Phase.
bat. bol.
Sat. Sol.
— 10
13.9 Ice
-40
69.7
HNO3.3H2O
— 20
22.9 "
—42 Eutec.
70.5
" +HN03.H20
-30
27.8 «
-40
72.5
HNO3.H2O
-40
3I-5 "
-38m.pt.
77-75
"
—43 Eutec.
32.7 "+HN03.3H20
-40
82.4
"
-40
34 . 1 HN03.3H20
-50
86.5
"
-30
40
-60
88.8
«
— 20
49.2
— 66.3 Eutec.
89-95
" +HN03
— 18 . 5 m. pt.
53-8
-60
91.9
HNO,
— 20
58.5
-5o
94-8
"
-30
65-4
—4i.2m.pt.
100
•
NITROGEN Na.
SOLUBILITY IN WATER.
(Winkler — Ber. 24, 3606, '91; Braun — Z. physik. Chem. 33, 732, 'oo; Bohr and Bock — Wied. Ann,
44, 318, '91.)
t°
L/oemcien
t 01 ADsorptic
A,
in p.
" Solubility " B'.
?•
0
0.0235*
...t
0.0233*
O.OO239*
5
0.0208
0.0215
0.0217
O.O2O6
O.OO259
10
0.0186
0-0196
O.O2OO
0.0183
0.00230
15
0.0168
0.0179
0.0179
0-0165
0.00208
20
0.0154
0-0164
O.Ol62
O.OI5I
0.00189
25
0.0143
O.OI5O
0.0143
0.0139
0.00174
30
0.0134
0-0138
. . .
O.OI28
o. 00161
35
0-0125
0.0127
. . .
O.OIlS
0.00148
40
0.0118
O-OIlS
O-OIIO
0.00139
50
0.0109
0.0106
. . .
0.0096
0-OOI2I
60
0.0102
O-OIOO
. . .
0.0082
O.OOIO5
80
0.0096
0.0051
0.00069
100
0.0095
o.oioo
o.oooo
o.ooooo
*w.
t B. and B.
tB.
For values of ft, ft', and q, see Ethane, p. 285.
Single determinations of the solubility of nitrogen in water reported by Hiifner
(1906-07), Bohr (1910), Muller (1912-13) and von Hammel (1915), are, on
the average, about 2-3 units in the fourth place higher than the above figures
of Winkler for the absorption coefficient ft. Drucker and Moles (1910), give an
extensive review of the literature and present results which, they state, are in very
satisfactory agreement with previous determinations. A critical review of the
literature of the solubility of nitrogen in water and in sea water is given by
Coste (1917).
Data for the solubility of the nitrogen of air in water are given by Fox (iQOQa).
The oxygen was removed from air and the solubility of the residual N + 1.185%
argon was determined. After making correction for the argon, the following
formula for the solubility of pure nitrogen in water was deduced :
1000 X coef. of abs. ft = 22.998 — 0.5298 1 -f 0.009196 £ — 0.00006779 **•
Data for the solubility of nitrogen in water at pressures up to 10 atmospheres
are given by Cassuto (1913). The solubility was found to increase at a some-
what slower rate than proportional to the pressure.
NITROGEN 458
SOLUBILITY OF NITROGEN IN SEA WATER.
(Fox, igoga).
Before using the sample of sea water for the solubility determinations it was
found necessary to add acid, otherwise the CO2 could not be boiled out or the
precipitation of neutral carbonates prevented. The very small amount of acid
was titrated back, using phenolphthaleine as indicator.
The results are in terms of number of cc. of nitrogen (containing argon) ab-
sorbed by 1000 cc. of sea water from a free dry atmosphere of 760 mm. pressure.
The calculated formula expressing the solubility is:
1000 a = 18.639 — 04304 1 + o-o°7453 ** — 0.0000549 &
— Q (0.2172 — 0.007187 / -f 0.0000952 12).
imorine t°-n° A°
r looo.
8°.
12
°.
16°.
20°.
24°.
28°.
O
18
-64
17.02
15.63
14.
45
13-45
12,
•59
11.86
11.25
4
17
•74
16.27
14.98
88
12.94
12
15
11.46
10.89
8
16
.90
15-51
I4.32
13.
30
12.44
II
,70
11.07
10.52
12
16
•03
14-75
13-66
12.
72
H-93
II
•25
10.67
10. 16
16
15
.18
14
13
12.
15
n-73
10,
,81
10.27
9.80
20
14
.31
13.27
12.34
II.
57
10.92
10,
36
9.87
9-44
A recalculation of Fox's determinations to parts per million, with correction
for vapor pressure, is published by Whipple and Whipple (1911).
SOLUBILITY OF NITROGEN IN AQUEOUS SOLUTIONS OF SULFURIC ACID
Results at 21°. (Bohr, 1910.) Results at 20°. (Christoff, 1006.)
Normality of Absorption Coef . Normality of Absorp. Coef. Per cent Ostwald Solubility
Aq. H2SO4. 0 (Bunsen). Aq. H2SO4. 0 (Bunsen). H2SO4. Expression 1M.
o 0.0156 24.8 0.0048 o 0.01537
4.9 O.009I 29.6 O.O05I 35-82 0.008447
8.9 0.0072 34.3 o.oioo 61.62 0.006144
10.7 0.0066 35-8* 0.0129 95-6 0.01672
20.3 0.0049
* = about 96%.
For definitions of Absorption Coef. (Bunsen) and Solubility Expression (Ost-
wald), see p. 227.
SOLUBILITY OF NITROGEN IN AQUEOUS SALT SOLUTIONS.
(Braun.)
Coefficient of Absorption of N in Barium Chloride Solutions of:
i .
13.83 Per cent
11.92 Per cent.
6.90 Per cent.
3.87 Per cent. 3.33 Per cent.
5
O.OI27
0.0137
0.0160
O.OlSo
0.0183
10
O.OII7
0.0125
0.0147
0.0166
0.0168
15
O.OI04
O.OII4
0.0132
0.0148
0.0150
20
0.0092
0.0098
0.0118
0.0132
0.0135
25
0.0078
0.0086
0.0104
O.OII4
0.0119
Coefficient of Absorption of N in Sodium Chloride Solutions of:
'
11.73 Per cent.
8.14 Per cent.
6.4 Per cent.
2.12 Per cent. 0.67 Per cent.
5
O.OIO2
O.OI27
0.0138
O.OI79
0.0200
10
0.0093
O.OII3
O.OI26
0.0164
0.0185
15
O.OOSl
O.OIOI
O.OII3
O.OI47
0.0l64
20
0.0066
0.0087
0.0098
O.OI3I
O.OI48
25
O.OO47
0.0075
0.0083
O.OII3
0.0130
SOLUBILITY OF NITROGEN IN ALCOHOL.
(Bunsen.)
t°. o°. 5°. 10°. 15°. 20°. 24°.
Vols. N * dissolved
by i Vol. Alcohol. 0.1263 0.1244 0.1228 0.1214 0.1204 0.1198
* At o° and 760 mm.
459
NITROGEN
SOLUBILITY OF NITROGEN IN MIXTURES OF ETHYL ALCOHOL AND WATER
AT 25°.
(Just, 1901.)
Results in terms of the Ostwald solubility expression, see p. 227.
Dissolved
Nfe).
0.01634
0.01536
Vol. % H2O in
Mixture.
Vol. % Alcohol'in
Mixture.
100
0
80
20
67
33
0
100 (99-8%
SOLUBILITY OF NITROGEN IN SEVERAL SOLVENTS AT 20° AND 25°.
(Just.)
Solvent. ^25.
Water 0.01634
Aniline o . 03074
Carbon Disulfide 0.05860
Nitro Benzene
Benzene
Acetic Acid
Xylene
Amyl Alcohol 0.1225
0.06255
0.1159
o. 1190
o. 1217
0.01705
0.02992
0.05290
0.06082
o. 1114
o. 1172
o. 1185
0.1208
Solvent. /25-
Toluene 0.1235
Chloroform 0.1348
Methyl Alcohol o. 1415
Ethyl Alcohol (99-8%) o. 1432
Acetone 0.1460
Amyl Acetate 0.1542
Ethyl Acetate 0.1727
Isobutyl Acetate o. 1734
*20.
O.II86
0.1282
0.1348
O.I40O
0.1383
o. 1512
0.1678
0.1701
SOLUBILITY OF NITROGEN IN PETROLEUM. COEFFICIENT OF ABSORPTION AT
10° = 0.135, AT 20° = 0.117.
(Gniewasz and Walfisz, 1887.)
SOLUBILITY OF NITROGEN IN AQUEOUS PROPIONIC ACID AND UREA
SOLUTIONS.
(Braun.)
Coefficient of Absorption of N in C2H5COOH Solutions of:
I/ .
11.22 per cent.
9.54 per cent.
6.07 per cent.
4.08 per cent.
3.82 per cent.
5
10
i5
20
0.0195
0.0178
'0.0159
0.0146
0.0204
0.0182
0.0l63
0.0147
0.0208
0.0186
0.0164
0.0148
O.O2IO
0.0192
0.0169
0.0154
O.O2O9
O.OI9I
O.Ol67
0.0155
25
0.0130
0.0134
0.0134
0.0137
0.0137
Coefficient of Absorption of N in CO(NHs), Solutions of:
15-65
per cent.
11.9 per cent.
9.42
per cent.
6.90 per cent.
5.15 per cent.
2.28 per cent.
5
10
i5
20
0.
O.
0.
0.
0175
Ol62
0150
OI4O
o
0
O
O
.0179
.0167
.0149
.0139
O,
o
o
o
OI9O
,0176
0158
,0146
0
O
0
0
.0198
.0183
.0165
.0151
0
O
0
0
.0197
.0182
•0165
.0151
0.0199
0.0l84
O.OI7I
0.0155
25
o.
0130
0
.0130
o
0133
O
.0137
0
•0135
0.0139
NITROGEN
460
SOLUBILITY OF NITROGEN IN AQUEOUS SOLUTIONS OF CHLORAL HYDRATE AT 15°.
Results by Miiller, C (1912-13.)
Gms.
Results by von Hammel (1915).
Gms.
CC1S.CH(OH),
</2o of Aq.
Absorp. Coef.
CC13CH(OH)2
Abs. Coef.
Solubility L*
per ioo Gms.
• Sol.
/Sat 15°.
per ioo Gms.
0 at 15°.
(Ostwald).
Aq. Sol.
Aq. Sol.
0
I
0.0170
0
0.0170
0.01796
15-8
1.0738
0.0158
15
0.0152
0.0160
28.2
I.I422
0.01422
26.1
O.OI4I
0.0149
37-25
I . 1946
O.OI3OO
37-6
0.0123
O.OI3O
47
1-2535
0.01275
48.9
O.OII5
O.OI2I
56.52
1.3225
O.OI245
61.3
O.OII4
O.OI2O
71.5
I.44I
0.01420
70.9
0.0131
0.0138
78.8
1.503
0.01492
79.1
0.0156
0.0165
SOLUBILITY OF NITROGEN IN AQUEOUS SOLUTIONS OF GLYCEROL.
Results of Miiller, C. Results of von Hammel Results of Drucker
(1912-13). (1915). and Moles (1910).
Gms. Gms. Gms.
IOO (
Aq.
Sol.'
1
1 '
ioo Gms.
Aq. Sol.
p
1 5 '
Aq- sSS'
25
.061
0
.01266
15-7
o
01400
0
0
0.0156
42
2
.108
0
.00976
29.9
o
01087
16
I.
0392
0.0103
51
5
•133
0
.00759
46.6
0
00840
29.7
I.
0744
0.0067
58
.151
0
.00703
57-6
o
00698
48.9
I.
1263
0.0052
80
25
.212
0
.00530
67.1
0
00635
74-5
I .
1931
0.0025
90
.240
o
.00583
77
0
00527
84.1
I.
2213
0.0024
95
.249
0
.00716
88.5
0
00536
99-25
0
00524
Solubility of Nz in pure isobutyric acid of fa = 0.9481, IM (Ost«vaH) = 0.1651.
(Drucker and Moles, 1910.)
Solubility of N2 in aq. 37.5% isobutyric acid of fa — 0.9985, 4s (Ostwald)
= 0.0396. (Drucker and Moles, 1910.)
Solubility of N2 in aq. 37.5% isobutyric acid of fa = 0.9985, ^ (Ostwald)
= 0.0384, (Drucker and Moles, 1910.)
SOLUBILITY OF NITROGEN IN AQUEOUS SOLUTIONS OF SEVERAL COMPOUNDS.
(Huiner, 1906-07.)
Cone, of Aq. Solution.
t°. Abs. Coef. 0.
Aq. solution 01:
Normality.
Gms. per Liter.
Glucose
I
180
"
0-5
90
"
O.25
45
Alanine (« Aminopropionic Acid)
I
89
GlyCOCol (Aminoacetic Acid)
I
75
Aribinose
I
150
Levulose
I
180
Erythritol
I
122
Urea
I
60
Acetamide
I
59
20.18
2O. 21
20.2
0.01215
0.01380
0.01480
2O.I9
20. 16
0.01213
O.OI2I2
2O. 21
O.OI203
2O.25
O.OI22I
20.25
20. l8
O.OI32I
0.01477
20.22
0.01475
SOLUBILITY OF NITROGEN IN AQUEOUS SOLUTIONS OF CANE SUGAR AT 15°.
(Miiller, C., 1912-13.)
per ioo Urns.
Aq. Solution.
11.38
2O
Abs. Coef.
at 15°.
Gms.
per ioo Gms.
Aq. Solution.
Aq. Sol.
I.I29
Abs. Coef. 0
at 15°.
Aq. Sol.
1.050 0.61480 30.12 I.I29 O.OIO90
1.082 O.OI280 47.89 1.220 0.00785
29.93 I.I28 O.OI053 48.57 1.223 0.00700
Data for the solubility of nitrogen in defibrinated ox-blood and ox serum under
pressures varying 760-1400 mm. Hg are given by Findlay and Creighton (1910-11).
Data for the solubility of nitrogen in liquid oxygen are given by Erdman and
Bedford (1904) and Stock (1904.)
46l
NITROGEN
SOLUBILITY OF NITROGEN IN METHYL ALCOHOL SOLUTIONS OF POTASSIUM
IODIDE AND OF UREA.
(Levi, 1901.)
Solubility of N (in terms of the Ostwald Solubility Expression /)•
Solvent.
Cms. KI or of Urea
At s°.
At 15°.
At 25°.
is of Solvent. /». du of Solvent. /u.
O %(=pureCH£)H)
2.152 KI
3-053 "
10.939 "
2.738 Urea
4.841 "
7-377 "
a* of Solvent. J*.
0.7937 0.1649
0.8019 0.1524
O.SlOI
0.8801
0.7997
0.8o8o
0.8350 0.1878 0.8241 O.l6oo 0.8193
O.8o8o 0.2154 0.7980 0.1923
0.8171 0.2028 0.8070 0.1802
0.1756
0.1464
0.2030
0.1951
0.8249 0.1966
0.8930 0.1676
0.8148
0.8231
0.8015
0.8841
0.8050 0.1823
O.8I22 O.I75O
0.1466
0.1258
O.I56l
O.I49I
0.1444
SOLUBILITY OF NITROGEN IN ETHYL ETHER.
(Christoff, 1912.)
Results in terms of the Ostwald expression / (see p. 227), IQ = 0.2580, /w = 0.2561.
WTTROGEN OXIDE (ic)
NO.
SOLUBILITY IN WATER.
(Winkler, 1901.)
t°.
0-
v.
?•
t°.
ft.
p.
g-
0
0.0738
0
•0734
O
.00984
40
0.0351
o
•0325
o
.00440
5
0.0646
0
.0641
0
.00860
50
0.0315
o
.0277
o
•00376
10
0.0571
o
.0564
o
•00757
60
0.0295
o
.0237
c
-00324
15
0.0515
o
.0506
0
.00680
70
0.0281
o
•0195
o
.00267
20
0.0471
o
.0460
o
.00618
80
0.0270
o
.0144
.0
.00199
25
0.0430
o
.0419
0
.00564
00
0.0265
o
.0082
o
.00114
30
0.0400
ro
.0384
o
•00517
100
0.0263
o
.0000
6
.00000
For values of /3, £' and q, see Ethane, page 285.
SOLUBILITY OF NITRIC OXIDE IN AQUEOUS SULPHURIC Aero SOLUTIONS
AT 18°.
(Lunge, 1885; Tower, 1906.)
(0.035,
Wt. per cent H*SO4
in Solution.
Sp.Gr.
at 15°.
98 ]
.84
00 ]
.82
80 ]
•733
70 . ]
.616
60 1
•503
50 ']
•399
Tension of Solubility Coefficient
HjO Vapor. of NO at iS°.
0.0227
O.I mm.
0.4 ;;
0.0193
0.0117
n
0.0113
0.0118
6.2 "
O.OI2O
(0.017, L.)
* Volume of NO (at 760 mm.) per i volume of aqueous HjSO4.
SOLUBILITY OF NITRIC OXIDE IN ALCOHOL.
(Bunsen.)
0°
0.316
5°
0.300
10"
0.286
15°
0.275
20°
0.266
24°
0.261
Vols. NO*
absorbed by i vol. Ale.
* At o° and 760 mm.
Data for the solubility of nitric oxide in aqueous solutions of FeSO4, NiSO4r
CoSO4 and MnCl2 at 20° are given by Usher (1908); Hufner (1907) and Man-
chot and Zecheulmayer (1906).
The abs. coef. 0 for N in sat. aq. NiSO4 at 20° is 0.0245; for sat. CoSO4 it is
0.0288 and for sat. aq. MnClj it is 0.0082.
NITROGEN OXIDE 462
NITROUS OXIDE N2O.
SOLUBILITY IN WATER.
(Bunsen; Roth, 1897; Knopp, 1904; Geffcken, 1904.)
Coefficient of Absorption ft
t * A
(B.)
(R.)
«.
(R.)
(K.)
(G.)
5
1.0954
I . 1403
0.205
1.161
. . .
- 1.067
10
0.9196
0-9479
0.171
0.9815
. . .
0.9101
15
0.7778
0.7896
0.143
0-8315
0.7784
20
0.6700
0.6654
O.I2I
0.7131
0.6739
0.6756
2^
0.5961
0.5752
O.IO4
0.6281
0.5942
* Calculated by Geffcken.
For definitions of /8 and g, see p. 285; for /, see p. 227.
NOTE. — Knopp and also Geffcken call attention to the fact that
Roth in making his determinations used a rubber tube between the
gas burette and the shaking flask, and give this as an explanation of
the high results which he obtained.
SOLUBILITY OP NITROUS OXIDE IN AQUEOUS SULPHURIC ACID.
(Lunge — Ber. 14, 2188, '81; see also Geffcken 's results.)
Sp. Gr. of H2SO4 1.84 i. 80 1.705 1.45 1.25
Vols. N2O dissolved
by loo vols. H2SO4 75.7 66.0 39.1 41-6 33.0
100 vols. of KOH solution of 1.12 Sp. Gr. absorb 18.7 vols. N2O.
100 vols. of NaOH solution of i.io Sp. Gr. absorb 23.1 vols. N2O.
SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF ACIDS.
(Geffcken.)
Results in terms of the Ostwald Solubility Expression (/). See p. 227.
In Hydrochloric Acid. In Nitric Acid. In Sulphuric Acid.
Cms. HCl N2O Dissolved Qms. HNO3 N2O Dissolved Gms. H2SO4 N2O Dissolved
per Liter. /16. /^ per Liter. /15. * fa. per Liter. ;18. J^
18.22 0.755 o-577 36.52 °-777 0.597 24.52 0.734 0.566
36.45 0.738 0.568 63.05 0.777 0.602 49.04 0.699 °-543
72.90 0.716 0.557 126.10 0.775 0.611 98.08 0.645 0.509
147.12 0.602 0.482
196.16 0.562 0.463
SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF:
(Roth.)
Phosphoric Acid. Oxalic Acid.
*•
s
10
^5
20
2$
Coefficient of Abs.
in H3PO4 Solutions of:
Coefficient of Abs. in
(COOH)2 Solutions of;
' 0.812%. 3-70%.
I.I450 I.I094
0.9526 0.9264
0.7940 0-7745
0.6694 0.6538
0.5784 0.5643
3-38%.
^OST
0.8827
0.7388
0.6253
0.5427
i
0
0
0
0
4.72%.
•0365
.8665
•7258
.6147
•5329
0
0
0
0
0
8.84%.
.9883
.8296
.6977
.5926
•5I43
9-89%.
0-9635
0.8101
0.6826
0.5810
0-5054
0
o
o
0
0
13.35%.
.9171
.7711
•6505
•5555
.4860
463
NITROUS OXIDE
SOLUBILITY OP NITROUS OXIDE IN AQUEOUS SOLUTIONS OP PROPIONIC
ACID AT 20°.
(Knopp.)
Cms. C2H5COOH
per liter *5-*5 60.42
Coef. of Absorp-
tion of N2O 0.6323 0.6369
158.4 176.6 344.0
0.6504 0.6534 0.7219
SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SALT SOLUTIONS.
Results by Geffcken
page 227.
Salt.
Ammonium Chloride
Ammonium Chloride
Caesium Chloride
Lithium Chloride
Lithium Chloride
Potassium Bromide
Potassium Bromide
Potassium Chloride
Potassium Chloride
Potassium Iodide
Potassium Iodide
Potassium Hydroxide
Potassium Hydroxide
Rubidium Chloride
Rubidium Chloride
in terms of the Ostwald expression (/). See
Cone, of Salt per Liter.
Solubility of N20.
ormu a.
Gram Equiv.
Grams.
/is-
fe
NH4C1
o-5
26.76
0.730
o-557
NH4C1
I .0
53-52
0.691
0.529
CsCl
o-5
84.17
0.710
0-544
LiCl
o-5
21.24
0.697
o-535
LiCl
I .0
42.48
0.623
0.483
KBr
o-5
59-55
0.697
o-536
KBr
I.O
119.11
0.627
0.485
KC1
o-5
37-3
0.686
0.527
KC1
i .0
74-6
0.616
o-475
KI
o-5
83.06
0.702
0.541
KI
I.O
166.12
0-633
0.492
KOH
o-5
28.08
0.668
0.514
KOH
I .0
56.16
o-559
0.436
RbCl
o-5
60.47
0.695
o-533
RbCl
I .0
120.95
0.625
0.483
Results by Knopp, in terms of the coefficient of absorption. See
page 227
Salt. Formula.
Potassium Nitrate KNO3
Sodium Nitrate NaNO3
Cone, of Salt
per Liter.
Coef. of Absorption
Normality.
Grams.
of N2O at 20°.
0.1061
10.74
0.6173
0.2764
27.94
0.60O2
0.5630
56-97
0-57*3
1.1683
118.2
0.5196
0.1336
n-37
o . 6089
0.3052
25-97
0.5876
0.6286
53-5o
0-5465
I .1200
95-30
0.4926
Results by Roth, in terms of the coefficient of absorption.
Grams NaCl per
100 Grams
Solution.
O.Q9
1. 808
3.886
5-865
Coefficient of Absorption of N2O at:
<?.
1.0609
1.0032
0.9131
0.8428
10°.
0.8812
0.8383
0.7699
0.7090
15°.
0-7339
0.7026
0.6495
0.5976
90°.
O.OIQI
0.5962
0.5520
0.5088
fi£?.
O.S363
0.5190
0-4775
0.4424
NITROUS OXIDE
464
SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SALT SOLUTIONS.
Results by Gordon in terms of coefficient of absorption. See p. 227.
Concentration of Salt.
Coefficient of Absorption
Grams per Gram
100 Grams Mols.
Solution. per Liter.
5-79 0.547
o
5°.
.819
10°.
0.697
0
15°.
•591
0
20°-
•500
9
.86
0
.964
o
.668
0.586
0
•509
0
•435
13
•99
i
.416
o
.510
0
.441
0
.380
0
.328
i
•35
0
•319
o
.986
0
.831
0
.700
0
•594
3
•85
0.928
0
.878
0
•743
0.629 0.536
ii
.48
2
.883
o
,606
0
.512
0
•437
0
•382
2
•37
O
.219
o
934
0
.792
0
.670
0
•569
5
.46
O
.521
o
795
o
.665
0
•557
0
•474
8
•56
O
.836
0
.646
o-555
0
•477
o
•4i5
5
.90
0.521
o
.766
o
.664
0
.561
o
.471
7
.66
O
.687
o
.708
0
.586
0
.488
0
.414
10
•78
O
•997
o
•569
0
.491
o
.417
0.346
4
.90
0
.676
0
.879
0
•751
0.643
o
•555
7
.64
I
•037
o
•799
0
•693
o
591 0.494
14
•58
2
.147
o
•654
0
•574
0
•500
0
•430
22
.08
3
.414
o
•544
o
•459
0
•390
o
•339
2
.62
o
•154
o
.986
0.831
0
.701
0
.605
4
.78
0.285
o
.918
0
•763
0
•637
0
•542
6
.20
I
.107
o
.800
x>
.682
0
•585
0
•509
8
.88
I
.614
o
.713
0
.603
0
0
•434
12
•78
2
•391
0
•634
0
•532
0
•449
0.386
5
.76
O
•427
o
.808
0.677
0
•584
0
•495
8
•53
O
.646
o
.692
o
•574
0
.482
0
.416
12
•44
O
•974
o
•559
0
.486
0
•417
o
•354
3
.31
O
•215
o
.928
0
.788
0
.671
0
•578
5
•73
o
-380
0
.848
0
.709
0
.610
o
13
.24
o
•939
o
.644
0
•547
0
•463
0
•39°
Salt.
Calcium Chloride
u
Lithium Chloride
a
Lithium Sulphate
Magnesium Sulphate
ii
Potassium Chloride
tt
n
(i
Potassium Sulphate
Sodium Chloride
tt
Sodium Sulphate
Strontium Chloride
a
SOLUBILITY OP NITROUS OXIDE IN ALCOHOL AND IN AQUEOUS CHLORAL
HYDRATE SOLUTIONS AT 2cr.
(Bunsen; Knopp — Z. physik. Ch. 48, 106, '04.)
In Alcohol (B.).
In Aq. Chloral Hydrate (K.).
Vols. N20
t °. (at o° and 760 mm.)
per i Vol. Alcohol.
Normality
C2HCl3O.H2O.
Cms.
C2HC13O.H20
per Liter.
Coef. of
Abs. of NjO.
0
4.178
0.184
30-43
0.618
5
3-844
0-445
73.60
0-613
10
3-541
0.942
155-8
0.596
IS
3.268
I .165
192.7
0.589
20
3-025
1-474
243-8
o-579
24
2.853
i .911
316.4
0.567
SOLUBILITY OP NITROUS OXIDE IN PETROLEUM.
ABSORPTION AT 10° = 2.49, AT 20°
COEFFICIENT OF
= 2. ii.
(Gniewasz and Walfisz — Z. physik. Ch. i, 70, '87.)
465 NITROUS OXIDE
SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF GLYCEROL AND OF UREA.
(Roth, 1897.)
Coefficient of Absorption of N2O in Glycerol Solutions of:
3.46 Per cent.
6.73 Per cent. 12.
12 Per cent.
16.24 Per cent.
5
i
.097
i
•055
O
•999
0
•959
10
0
.917
0
.887
0
.841
O
.810
*5
0
.767
0
•745
0
.710
o
.686
20
0
.647
0
.630
0
.605
0
•58S
25
0
•556
o
•542
0
•527
o
•508
Coefficient of Absorption of N2O in
Urea Solutions of:
3.31 per cent.
4.97 per cent.
6.37 per cent.
7.30 per cent.
9.97 per cent.
I
.104
I .
096
i. 088
I .IOI
1.069
0
.921
o.
92O
0.909
0.921
o.
901
0
.771
o.
773
0.761
0.772
o.
76l
o
•653
o.
6S6
0.644
0-655
o.
65*
0
•569
o.
567
0-559
0.570
o.
5<*>
5
10
15
20
25
SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF GLYCEROL.
(Henkel, 1905, 1912.)
Results at 15°. Results at 20°.
Per cent Glycerol. Absorption Coef. a. Per cent Glycerol. Absorption Coef. a.
o 0.7327 o 0.6288
2.49 0.7181 2.36 0.6131
3.28 o\7io3 4.88 0.5993
7.17 0.6844 6.88 0.5903
10.52 0.6668 9.86 0-5633
14.05 0.6410 15.82 °-53I5
17.08 0.6229
Data for the influence of colloids and fine suspensions on the solubility of ni-
trous oxide in water at 25° are given by Findlay and Creighton (1910), and Find-
lay and Howell (1914).
Results for solutions of ferric hydroxide, dextrin, arsenious sulfide, starch,
gelatin, glycogen, egg albumen, serum albumen, silicic acid and suspensions of
charcoal and of silica are given.
Data for the solubility of nitrous oxide in blood are given by Siebeck (1909)
and by Findlay and Creightonf (1910-11). •
NITROGEN TETROXIDE NO2.
Data for the solubility of nitrogen tetroxide in ferrous bromide solutions are
given by Thomas (1896).
Freezing-point data (solubility, see footnote, p. i), are given for mixtures
of NO2 + NO by v. Wittorff (1904), and for mixtures of NO2 + o Nitrotoluene
by Breithaupt.
NITROCELLULOSE (Soluble Pyroxylin, Tetra and Penta Nitrate).
SOLUBILITY IN ETHER-ALCOHOL MIXTURES.
(Matteoschat, 1914; see also Stepanow, 1907.)
A sample of gun cotton containing 12.95% N was used. The compound was
first covered with alcohol and then the amount of ether to yield the desired com-
position of solvent was added. Lower results were obtained with ready prepared
ether-alcohol mixtures.
Ratio of Gms. Gun Cotton Dissolved per 100 Cms. Solution in Mixtures Prepared with:
r : Alcohol.
99-5 Vol. % Alcohol.
95 Vol. % Alcohol.
90 Vol. % Alcohol.
80 Vol. % Alcohol.
i : 2
34-4
i : i
52-3
42-3
28.7
14.2
2 : i
40.5
52-4
53-9
45
3:1
25
42.4
53
57-5
NOVOCAINE 466
NOVOCAINE (base) CH2(C6H4NH2COO)CH2[N.(C2H6)2].2H2O.
100 cc. H2O dissolve 0.333 gm- anhydrous novocaine at 20°. (Zalai, 1910.)
100 cc. oil of sesame dissolve 4.29 gms. anhydrous novocaine at 20°.
NOVOCAINE (Hydrochloride) CH2(C6H4NH2COO).CH2[N(C2H6)2].HC1.
loo gms. H2O dissolve about 100 gms. of the salt at room temp.
100 gms. alcohol dissolve about 3 gms. of the salt at room temp.
OCTANE CH3(CH2)6CH3.
RECIPROCAL SOLUBILITY OF OCTANE AND PHENOL.
(Campetti and Del Grosso, 1913.)
AC Gms. Phenol per ^ 0 Gms. Phenol per
loo Gms. Mixture. 100 Gms. Mixture.
22.55 13.28 49.501!. t. 52.2
37.85 22.74 49.35 52.37
38-15 23-S3 44.7 7i-i4
44.70 32.85 30.65 82.01
47-75 41-72 19-65 85.99
OLEIC ACID C8Hi7CH:CH(CH2)7COOH.
SOLUBILITY OF OLEIC ACID IN AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1910.)
Oleic acid of d<& = 0.8935 and containing 99.5% acid, determined by titration,
was used. It was found that the addition of as little as one drop of this acid
to aq. alcohol solutions containing up to 50 wt. % C2H6OH caused an opalescence
on shaking, therefore, indicating a solubility of less than about 0.05 gm. acid per
100 cc. water or of aq. alcohol. With solutions containing more than 50 wt. %
C2H6OH the following results were obtained:
Wf Pot- , cc- Oleic Acid per
r w nw I0° cc- Aq. Alcohol to Remarks.
CjHjUH. produce cloudiness.
51 O . 08 — 0 . 2 Cloudiness gradually increased.
58.2 0.2 —0.4
65 -5 ' O . 3 — 0 . 6 Cloudiness disappeared when about 5.5 cc. acid had been added.
70.2 O.6 — I " " " " 4-5 cc. " " "
81.4 CO No cloudiness appeared at all.
It was found that although the end points obtained by addition of oleic acid
to aq. alcohol mixtures are not sharp, they become so when the procedure is
changed to addition of H2O*to mixtures of oleic acid and alcohol. By this method
perfectly clear liquid may be transformed by one drop of the H2O to an opa-
lescent mixture which, after standing a few minutes, separates into two liquid
layers. Determinations made in this way gave the following observed and cal-
culated quantities.
Gms. of Constituents to Yield Results Calculated from the
Opalescent Mixtures. Plotted Curve.
Alcohol + Oleic Acid Mixture. H2O Added Wt. Per cent cc. Oleic Acid Gms. Oleic Acid
to Cause Qh^OH in per 100 cc. per 100 Gms.
CjH6OH. Oleic Acid. Separation. Aq. Alcohol. Aq. Alcohol. Sat. Sol.
15.30 1-794. 10.4 57 ••• o
15-30 3-588 10.2 58.5 o 5
15.30 4.485 9.8 60 n 12.3
I5-3° 7-175 9-25 62.5 30 20
15.30 n. 210 8.05 65 49 3°-5
24.42 22.420 10.10 67.5 69 40
15.30 20.810 6.50 70 91 50
1.195 8.969 0.321 75.5 ... 68.5
80 ... 88
Alter standing 24 hours the opalescent mixtures separated into layers which
on analysis, gave the results shown in the following table:
467 OLEIC ACID
COMPOSITION OF UPPER AND LOWER LAYERS OBTAINED BY THE ADDITION OF
WATER TO MIXTURES OF AQUEOUS ALCOHOL AND OLEIC ACID AT 25°. (Con.
from p. 466).
Composition of Original Mixture. After Separation into Two Layers:
rwt. % *
cc. Aq.
cc.
cc. H2O Lower Layer.
Upper Layer.
in Aq.
Ale. Used.
Alcohol
Mixture.
Oleic
Acid.
to Cause / *
Separa- cc. Total
tion. Vol.
Sp. Gr.
cc. Oleic
Acid.
cc. Total
Vol.
Sp. Gr.
cc. Oleic
Acid.
70.2
25
2
3-9°
29
0.893
1.48
I
0-35
70.2
25
4
3-70
26
0.890
1.89
6
0.875
1.98
65.5
26.5
5
1-75
22.7
0.891
i-93
9-3
0.875
2.78
70.2
25
8
2-75
16
0.893
0.98
19
0.876
6-59
70.2
25
12.5
1-55
6
0.890
0.37
33-2
0.878
11.87
70.2
35
. 25
i
4-5
. 1 1
0.28
55-5
0.877
f
24.14
50 cc. Aq. Alcohol
50 cc. Benzine Layer.
Dist. Coef.
Layer.
Layer.
0.277
0.723
2.6l
O.II2
0.888
7-93
0.025
o-97S
39
O.OO6
0.994
166
0.002
0.998
499
The C2H5pH in the two layers could not be determined on account of excessive
foaming during distillation of the neutralized solution. Some losses occurred
in transferring the original mixtures to the graduated cylinders and differences
between final amounts and those originally present are due to these losses.
SOLUBILITY OF OLEIC ACID IN AQUEOUS SOLUTIONS OF BILE SALTS.
(Moore, Wilson and Hutchinson, 1909.)
<""-. ^iS'tr100
Water less than o . i
5% Aq. Solution of Bile Salts about o. 5
5% Aq. Solution of Bile Salts-f-i % Lecithin . 4
DISTRIBUTION OF OLEIC ACID BETWEEN AQUEOUS ALCOHOL AND BENZINE. (Holde.'io.)
Strength of Aq. Gm. (Approx.) of Oleic Acid in;
Alcohol in Vol.
Per cent.
84.1
76.9
63.7
50.5
42.4
SOLIDIFICATION-POINTS OF MIXTURES OF OLEIC AND STEARIC ACIDS. (Meldrum, '13.)
Solidification
Temp.
O
IO
20
30
4O
Additional data for the above system as well as for mixtures of oleic and
palmitic acids and for the ternary system oleic, palmitic and stearic acids are
given by Carlinfante and Levi-Malvano (1909). Results for Oleic Acid + Stearic
acid are also given by Fokin (1912).
TriOLEIN (C18H33O2)3C3H5.
SOLIDIFICATION- POINTS OF MIXTURES OF TRIOLEIN AND OTHER FATS.
(Kremann and Schoulz, 1912.)
Triolein + Tripalmitin. Triolein + Tristearin. Tripalmitin + Tristearin.
t°. Wt. Per cent f0 Wt. Per cent. f <, Wt. Per cent
Triolein. Triolein. . Tristearin.
— 7 loo +28 95.2 60.4 90
+25 93-9 44 85.3 58 75
48.2 78.5 50.7 76.7 57.8 . 69.4
50 73.9 56 68.8 56 60.2
56.9 53 64-3 47-2 57.2 53
60.9 27.2 64.3 25.4 55.1 43-8
62.6 o 56 o 54.5 31.2
60 . 4 8.4
Data for the ternary system, triolein. tripalmitin and tristearin are also given.
Per cent Oleic Aci'd
Solidification
Per cent Oleic Acid
in Mixture.
Temp.
in Mixture.
54-8
50
44-7
53-3
60
41.2
51-6
70
36.6
49-7
80
30-5
47.6
OILS
468
OILS. (See also Fats, p. 302.)
SOLUBILITY OF SEVERAL OILS IN ALCOHOL (di5 = 0.795) AT I4~I50-
(Davidsohn and Wrage, 1915.)
f)-i Gms. Oil per 100 Gms.
Sat Sol.
Linseed Oil 3.32
Rape Oil i . 36
Cotton Seed Oil 3.61
Olive Oil 2.25
Results are also given for the solubility of mixtures of oils and fatty acids in
alcohol. The following results at 22°, in terms of approx. volume of oil dissolved
by 100 volumes of 80% alcohol, are given by Aubert (1902). Nigella oil, 4.3;
oil of boldo leaves, more than 100; matico oil, about 20; cascarilla oil, 5; weld-
mint oil, 66.
^ Miscibility curves for various oils with acetone, petroleum and aniline are
given by Louise (1911). The use of this data for the identification of oils and
the detection of adulterants in them is described.
An extensive series of observations on the solubility of water in oils and on the
water content of various oils is given by Umney and Bunker (1912).
Freezing-point data for oil of helianthus annus + stearic acid are given by
Fokin (1912).
OSMIC ACID OsO4, 100 gms. H2O dissolve 5.88 gms. Osmic Acid at about 15°.
(Squire and Caines, 1905.)
OXALIC ACID H2C204.2H20.
SOLUBILITY IN WATER.
(Koppel and Cahn, 1908; for older* data see Alluard, Miczynski, 1886; Lamouroux, 1899.)
— 0.064
0.1805
— 0.152
0.452
- 0.533
I. -820
- 0.936
3.291
- i.5o
5.836
- o.9S
3.302
o
3.416
+ 10
- 5.731
Ice 20 8.69 HjQC^HjO
30 12.46
40 17.71
50 23.93
60 30. 71
70 37.92
80 45 . 80
90.2 54.67 "
H2C2O4.2H2O melts in its H2O of crystallization at 98°.
SOLUBILITY OF OXALIC ACID IN AQUEOUS HC1.AND IN AQUEOUS HNO3 AT 30°.
(Masson, 1.912.)
In Aq. Hydrochloric Acid.
In Aq. Nitric Acid.
G. Mols.
G. Mols.
Gms.
G. Mols.
G. Mols.
Gms.
HC1 <*™Sat.
(COOH)2
(COOH)2
HNO3 <
fag Sat.
(COOH)2
(COOH)2
per liter Sol
per liter
per liter
per liter
Sol.
per liter
per liter
Sat. Sol.
Sat. Sol.
Sat. Sol.
Sat. Sol.
Sat. Sol.
Sat. Sol.
0
-0594
1.479
I33-I
0.478 1.0648
1.268
114. 1
0.503
• 0561
I.I90
107.1
I. 606 1.0932
1.039
93.48
0.970
•0577
1.032
92.85
4.224
.1666
0.790
71.09
1-939
.0654
0.821
73-88
9-590
•3074
0.639
57-50
2-959
•0757
0.675
60.74
13.62
•3938
0.847
76.23
4-528
•0957
0-555
49-95
14.12
.4060
0.966
86.94
6.026
.1165
0.525
47-25
15-59
•43J9
1 . 114
IOO. 2
7.907
.1494
0.607
54.63
16.92
•4443
0.840
75-6
9.680
. 1843
0.871
78.38
20.84
.4819
0.524
47-iS
21.63 L49I7
0-553
49.76
SOLUBILITY OF OXALIC ACID
IN AQUEOUS
SOLUTIONS OF H2SO4 AT 25°.
(Wirth, '08.)
ACQ0nHS°o ^°'fSat-
Gms. per 100 Gms. Sat. Sol.
Cone, of 3
An TT ^O ***
B of Sat Gms' per I0° Gms' Sat' Sol-
No*rrnSuy4. So1'
S03.
(COOH)2.
Aq. Xlgov^
Normality.
5 Sol.
S03.
(COOH)2.
o 1.047
O
10.23
4.85
I-I57
14
3-92
I I . 064
2.98
8.03
5.67
I.I77
16.44
3-51
2 . 39 i . 140
7.30
6.02
6-45
1.220
17.84
3.12
4.36 1.146
12.57
4.26
8.9
1.280
25.92
2-37
469 OXALIC ACID
SOLUBILITY OF OXALIC ACID IN SEVERAL ALCOHOLS.
(Timofeiew, 1894.)
Gms. (COOH), Gms. (COOH),
Alcohol. t°. per zoo Gms. Alcohol. t°. per 100 Gms.
Sat. Sol. Sat. Sol.
Methyl Alcohol
— 1.5
34-2
Propyl Alcohol — 1.5
12.2
« «
+ 20.2
39-8
+ 18.5
16.7
Ethyl Alcohol
- i-5
22.4
20.2
« a
+ I8.5
26.2
Isobutyl Alcohol 20 . 2
10.9
u tt
20.2
26.9
SOLUBILITY OF OXALIC ACID IN ABSOLUTE AND IN AQUEOUS ETHER AT 25°.
(Bodtker, 1897; Bourgoin.)
100 gms. absolute ether dissolve 1.47 gms. (COOH)2.2H2O.
100 gms. absolute ether dissolve 23.59 gms. (COOH)2.
In Aqueous Ether Solutions.
Gms. Solid Acid Added per 100 cc. Ether Solution. Gms. per 100 cc. Ether Solution.
(COOH)2.2H2O. (COOH)2. HA (COOH)2/
(1) 5 o 1.250 0.742
(2) 5 o 0.788 0.720
5 o 0.418 1.044
5 2.44 0.360 3.388
5 4.82 0.484 6.038
5 7-i4 0.558 8.538
5 9.42 0.632 10.996
5 11-63 0.676 13-316
5 13-79 0.760 15.684
5 18.18 0.816 17.818
5 22.73 0.816 17.818
(i) Ether saturated with water. (2) Ether containing 0.694 Per cent water.
100 gms. glycerol dissolve 15 gms. oxalic acid at 15.5°. (Ossendowski, 1907.)
loo gms. 95% formic acid dissolve 9.74 gms. anhydrous oxalic acid at 16.8°.
(Aschan, 1913.)
DISTRIBUTION OF OXALIC ACID BETWEEN WATER AND AMYL ALCOHOL AT 20°.
(Herz and Fischer, 1904.)
Millimols \ (COOH)2 per 10 cc. Gms. (COOH)2 per 100 cc.
Aq. Layer. Alcoholic Layer. Aq. Layer. Alcoholic Layer.
O.68o6 0.1451 0.306 0.0653
2.364 0.7233 1.064 0.326
6.699 2.550 3.015 1.148
10.029 4-300 4-5H 1-934
Data for the distribution of oxalic acid between mixtures of amyl alcohol +
ether and water at 25° are given by Herz and Kurzer (1910).
DISTRIBUTION OF OXALIC ACID BETWEEN WATER AND ETHER.
(Pinnow, 1915.)
Results at 15°. Results at 27°.
Gm. Mols. (COOH)2 per Liter. Dist. Coef. of: Gm. Mols. (COOH)2 per Liter. Dist. Coef. of;
Water
Ether
Total
Undissoc.
Water
Ether
Total
Undissoc.
Layer.
Layer.
Acid.
Acid.
Layer.
Layer.
Acid.
Acid.
0-3435
O.O2945
II
.6
8.
49
O,
,760
0.0637
II
9
8.18
0.1885
0.01395
13
•5
8.
81
0,
56l
0.0433
13
8-37
O.I24
0.00845
14
.8
8.
69
O
3575
0.025O
14
3
8.26
0.0892
0.00553
16
.1
8.
72
O
2550
0.0165
15
5
8.12
o . 0470
0.00248
19
8.
19
0.
1754
0.01025
17
i
7.94
0.0435
O.OO22
19
.8
8.
26
Data for the effect of H2SO4 upon the above distribution are also given.
Data similar to the above for a greater range of cone, at 25° are given by
Chandler (1908).
OXYGEN
470
OXYGEN 02.
SOLUBILITY IN WATER.
*«. Coef. of Absorption /9. g.
(Winkler, 1891; Bohr and Bock, 1891.)
0
0.0489*
0.0496!
5
0.0429
0.0439
IO
0.0380
0.0390
15
0.0342
0.0350
20
0.0310
0.0317
25
0.0283
0.0290
30
o. 0261
0.0268
0.00695
0.00607
0.00537
0.00480
0.00434
0.00393
0.00359
*w.
For values of /3 and q see Ethane, p. 285.
cc. 0 per
Liter H2O.
10.187
8.907
7.873
7.038
6.356
5.776
5-255
t°.
40
50
60
70
80
90
IOO
Coef. of Absorption /5. ?.
O.
0.
O.
0.
0.
0.
0.
0231*
0209
0195
0183
0176
OI72
OI7O
0.0233!
o. 0207
0.0189
0.0178
0.0172
0.0169
0.0168
0.
o.
0.
o.
0.
0.
0.
00308
00266
00227
00186
00138
00079
ooooo
t B. and B.
According to determinations by Fox (igoga), which agree satisfactorily with the above, the solubility
of oxygen in water is expressed by the formula:
1000 X abs. coef. ft = 49-239 — i-344° < + 0.28752 ft — 0.0003024 fl.
References to more recent papers on the solubility of oxygen are given by Coste (1917, 1918).
SOLUBILITY OF THE OXYGEN OF AIR IN WATER.
t°. 5-2°. 5-65°. 14-78°.
Solubility* 8.856 8.744 7.08
* cc. Oxygen per 1000 cc. H2O saturated with air at 760 mm.
24-8°.
5.762
SOLUBILITY OF OXYGEN IN WATER AND IN AQUEOUS SOLUTIONS OF ACIDS,
BASES AND SALTS. (Geffcken, 1904.)
Concentration per Liter.
Solubility of Oxygen.*
Water alone
Hydrochloric Acid
Nitric Acid
Sulphuric Acid
Potassium Hydroxide
Sodium Hydroxide
Potassium Sulphate
Sodium Chloride
Gram Equiv,
, Grams.
o-5
18.22
I-O
36-45
2.0
72.90
o-5
36.52
i.o
63-05
2.O
I26.IO
o-5
24.52
I.O
49.04
2.0
98.08
3-o
I47-I2
4.0
196.16
5-o
245 . 20
o-5
28.08
I.O
56.16
o-5
20.03
I.O
40.06
2.0
80. 12
o-5
43-59
I.O
87.18
o-5
29.25
I.O
58.5
2.0
119.0
In terms of the Ostwald Solubility Expression.
0.0363
0.0344
0.0327
0.0299
0.0348
0.0336
0.0315
0.0338
0.0319
0-0335
0.0256
0.0233
0.0213
0.0291
0.0234
0.0288
0.0231
0.0152
0.0294
0.0237
0.0308
.0.0260
0.0182
See page 227.
0-0308
0-0296
0.0287
0-0267
0.0302
0.0295
0-0284
0.0288
0.0275
0.0251
0.0229
o . 0209
O.OI94
O.O252
O.O2O6
0.0250
0-0204
0.0133
0.0253
O.O2O7
O.O262
0.0223
0.0158
SOLUBILITY OF OXYGEN IN AQUEOUS POTASSIUM CYANIDE SOLUTIONS AT 20°.
(Maclaurin, 1893.)
Cms. KCN per ioo gms. sol. i 10 20
Coefficient of absorption j3 0.029 0.018 0.013
30
0.008
5<>
0.003
471
OXYGEN
SOLUBILITY OF OXYGEN IN SEA WATER.
(Fox, igoga.)
Before using the sample of sea water for the solubility determinations, it was
found necessary to add acid, otherwise the COZ could not be boiled out or the
precipitation of neutral carbonates prevented. The very small amount of acid
was titrated back, using phenolphthaleine as indicator.
Results in terms of cc. of oxygen absorbed by 1000 cc. of sea water from a
free dry atmosphere at 760 mm. pressure.
The calculated formula expressing the solubility is: 1000 a = 10.291 — 0.2809 t
-f- 0.006009 P + 0.0000632 P — Cl (0.1161 — 0.003922 / + 0.0000631 £).
Parts Chlorine
per 1000.
t° =
o°.
4°-
8°.
12°.
16°.
20°.
24°.
28°.
O
IO.
29
9
.26
8.40
7.68
7.08
6-57
6.
14
5-75
4
9-
83
8
•85
8.04
7.36
6.80
6-33
5-
9i
5-53
8
9-
36
8
•45
7.68
7.04
6.52
6.07
5-
67
5-3i
12
8.
90
8
.04
7-33
6.74
6.24
5-82
5-
44
5-08
16
8.
43
7
.64
6.97
6-43
5-90
5-56
5-
20
4.86
20
7-
97
7
•23
6.62
6. ii
5-69
5-31
4-
95
4.62
A recalculation of Fox's determinations to parts per million, with correction
for vapor pressure, is published by Whipple and Whipple (1911).
Additional data on the solubility of atmospheric oxygen in sea water are
given by Clowes and Biggs (1904).
Data for the solubility of oxygen in water under pressures up to 10 atmos-
pheres are given by Cassuto (1913). The solubility increases at a somewhat
slower rate than proportional to the pressure.
SOLUBILITY OF OXYGEN IN AQUEOUS SALT SOLUTIONS AT 25°.
(MacArthur, 1916.)
Aq. Salt
Solution.
da Aq.
Solu-
tion.
cc. oxy-
gen per
Liter.
Aq. Salt
Solution.
dK Aq. cc. Oxy-
Solu- gen per
tion. Liter.
Aq. Salt
Solution.
du ot cc. Oxy-
Solu- gen per
tion. Liter.
Dist. H20
I
5-78
0.25
ttKBr
1.019
5-29
O.I25« NaBr
1.007
5-65
O.I25» I1
JH4C1
I.OOI5
2.31
2
n "
1.079
3.27
0.25
n '
1.017
5-52
0.25 n
"
1.0025
1.16
4
n "
1.162
1.84
0.50
n "
1.036
5-15
i n
"
1.014
0.07
O.I25WKC1
1.003
5-52
I
n "
1.075
4-47
O.I25« BaCl2
1.019
540
0.25
n "
1. 0086
5-30
2
n "
1.150
3-37
0.25 n
"
1.042
5-04
0.50
n "
I.O2O
4.98'
3
n "
1.219
2-57
0.50 n
"
1.082
4.27
I
n "
I.O42
4.26
4
n "
I'3°5
2.O2
i n
"
I.I77
3.10
2
n "
1.086
3.21
6
n "
1-455
1.28
0.25 nCaCl,
1.022
S-o8
3
n "
I.I34
2.36
O.l25«NaCl
I.OO22
5.52
i n
"
1.084
3-71
4
n "
I.I70
1.86
0.25
n "
1.0067
5-30
5 n
"
1.34
2.14
O.I25«KI
I.OI3
5.65
0.50
n "
I.OI7
4.92
0.l25«CsCl
I.OI4
5.67
0.25
n '
I.O27
549
I
n "
1.038
4.20
o.i25«LiCl
I.OOO4
5.63
0.50
n '
1.056
5-20
2
n "
1.075
3.05
0.50 n
"
I.OO9I
I
n '
1.116
4-75
3
n "
1. 112
2.24
i n
"
I. O2 1
4-59
2
n '
1.23
3-77
4
n "
I.I49
1.62
2 n
«
1.044
3-63
5
n '
1.46
1.81
O.I25W Na2SO4
I.OI4
5.04
3 w
«
I.II3
1.97
0.25
MKNO,
1.015
5-49
0.25
n "
1.032
4.60
4 w
"
1.220
1. 12
0.50
n "
1.029
S-ii
0.50
n "
1.063
3-97
o.i25wMgCl,
1. 01 1
5.35
I-
n "
1.059
4.61
I
n "
I.I30
3
0.50 w
«
1.044
4.37
2
n "
i. no
3.65
0. 1 25« Sucrose
I.OI5
540
i n
i
1.085
o.i25« K2.SO4
1.016
0.25
n "
1.033
4.82
2 «
i
1.160
2.22
0.25
n "
1.032 .
4*.66
0.50
n "
i -6-i
1-39
4 n
•
1.284
0.78
0.5
n
i. 060
3.89
I
n "
1.147
3-20
5 **
'
1.343
0-54
o.i25»RbCl
1.0094
5.65
2
n "
1.336
1.84
OXYGEN 472
SOLUBILITY OF OXYGEN IN AQUEOUS SULFURIC ACID SOLUTIONS.
Results at 21°. (Bohr, 1910.) Results at 29°. (Christoff, 1906).
Normality of
H2S04.
Absorp.
Coef . ft.
Normality of
H2SO<.
Absorp.
Coef.0.
Wt. % Ostwald Solubility
H2SO4. Expression /jo-
0
0.0310
24.8
O.OI03
0
0.03756
4.9
0.0195
29.6
O.OII7
35-82
0.0l8l5
8.9
0-0155
34-3
0.0201
61.62
0.01407
10-7
0.0143
35. 8 (=96%)
0.0275
95.60
0.03303
20.3
O.OII9
SOLUBILITY OF OXYGEN IN ETHYL ALCOHOL, METHYL ALCOHOL AND
IN ACETONE.
(Timofejew — Z. physik. Ch. 6, 151, 'oo; Levi — Gazz. chim. ital. 3it II, 513, 'ox.)
O
5
10
15
20
25
30
40
SO
For values of ft and /3', see Ethane, p. 285. / = Ostwald Solubility Expres-
sion. See p. 227.
The formulae expressing the solubility of oxygen in methyl alcohol and in ace-
tone as shown in the above table are as follows:
In Methyl Alcohol / = 0.31864 — 0.002572 / — 0.00002866 ^.
In Acetone / = 0.2997 — 0.00318 / — 0.000012 P.
The formula expressing the absorption coefficient of oxygen in ethyl alcohol
is 0 = 0.23370 — 0.00074688 t + 0.000003288 P.
SOLUBILITY OF OXYGEN IN AQUEOUS ALCOHOL AT 20° AND 760 MM.
(Lubarsch,
i Ethyl Alcohol of 90.7% (T.).
In Methyl
Alcohol (L.)
In Acetone (L.)
0.
£'•
0.2337
0.2297
0.31864
0.2997
0.2301
0.2247
0-30506
0.2835
O.2266
0.2194
o . 29005
. 0-2667
0.2232
0-2137
0-27361
0.2493
0.2201
0.2073
0-25574
0-2313
0.2177 (24°)
0.2017 (24°)
0.23642
O.2I27
. . .
0.21569
0-1935
. . .
. . .
0.16990
0-1533
0.11840
0.1057
Wt. Per cent Vol. Per cent Wt. Per cent Vol. Per cent Wt. Per cent Vol. Per cent
Alcohol. Absorbed O. Alcohol. Absorbed O. Alcohol. Absorbed O.
o 2.98 23.08 2.52 50 3.50
9.09 2.78 28.57 2.49 66.67 -4-95
16.67 2-63 33 -33 2.67 80 5.66
SOLUBILITY OF OXYGEN IN PETROLEUM. COEFFICIENT OF ABSORPTION AT
10° = 0.229, AT 2O° = 0.202.
(Gniewasz and Walfisz, 1887.)
SOLUBILITY OF OXYGEN ETHYL ETHER.
(Christoff, 1912.)
Results in terms of the Ostwald Solubility Expression, A> = 0.4235, lw =*
0.4215.
473
OXYGEN
SOLUBILITY OF OXYGEN IN AQUEOUS SOLUTIONS OF:
Chloral.Hydrate at 20°.
(Muller, 1912-13.)
Glycerol at 15°. (Muller, 1912-13.)
Gms.
CC13.CH(OH)2
per loo Gms.
Aq. Sol.
Aq?Sok
ArBun°e^ ft (CH2OH)TcHOH d of
(Bunsen) IQQ Qms A Sol
at 20 • Aq. Sol.
Abs. Coef. 0
(Bunsen)
at 15°.
16.9
1.0798
0.02795
20.5
rfl2.5 =1.0509
O.O2742
32
1.1630
0.02495
25
dtf =
.0621
0.02521
52.9
1.2935
0.02325
37-3
dn* =
•0957
0.02022
61.08
1-354
O.O24IO
45
^12-5 =
.Il6l
O.OI744
65.5
1.382
0.02580
52
fi?12 -5 =
•I35I
O.OI57O
71.4
1.4404
0.02730
7i.5
dl2-b =
.1908
0.00950
78
1.46
0.03280
88.5
(/13.5=1.236
0.00886
SOLUBILITY OF OXYGEN IN AQUEOUS SOLUTIONS OF:
Glucose at 2O°. (Muller, 1912-13-)
Cane Sugar at 15°. (Mttlkr, 1912-13-)
Gms C H O
Abs, Coef. 0
Gms. QaHaOu
Abs. Coef. 0
per zoo Gms.
Aq. Sol.
dzo of
f Aq. Sol.
(Bunsen)
at 20°.
per 100 Gms.
Aq. Sol.
AqU Sol.
(Bunsen)
at 15°.
10.84
I.04I3
0.02690
12. 1
.1.0482
0.02969
20-7
1.0835
O.O225O
24.38
I. 1022
0.02396
33-8
I.I370
0.0l8l5
28.44
I.I205
o. 02181
1.2295
0.01390
42.96
I.I938
0.01600
58.84
I . 2649
0.01250
50
I.23I8
0.01359
INFLUENCE OF ANESTHETICS UPON THE SOLUBILITY OF OXYGEN IN OLIVE OIL.
(Hamberger, 1911.)
Name and Cone, of Solubility of Oxygen in;
Narcotic Added pure Narcotic
to the Oil. Solvent. Solution.
Sulfonal (0.8 per 100) 9 . 69 4.55
9.69
9.69
(saturated)
Trional
Tetronal (2 per 100)
«
Camphor (10 per 100)
9. 10
9. 10
9.67
9.67
8-53
5-68
6.25
4-55
5-68
9. 10
9. 20
7.96
Name and Cone, of
Narcotic Added
to the Oil. .
Monochlorhydrine (5
" ' (2-5
(1.25
(10
(5
(5
(2.5
D ichlorhy drine
«
Phenylurethan
Solubility of Oxygen in;
Pure Narcotic
Solvent. Solution,
penoo) 9.10 7.50
) 9.10 7.50
) 9.10 7.90
) 9.10 7.96
) 9.10 8
) 8.53 6.25
) 8.53 7.50
Data for the solubility of oxygen in liquid air are given by Baly (1900).
Data for the solubility of oxygen in hemoglobin are given by Jolin (1889).
Data for the solubility of oxygen in defibrinated ox-blood and ox-serum, at
pressures varying from 760 to about 1400 ram. Hg, are given by Findlay anc
Creighton (1911).
OZONE 03.
SOLUBILITY IN WATER.
(von Mailfert, 1894; Carius; Schone, 1873.)
t°.
w.
G.
R.
t°.
w.
G.
R.
0
39-4
61.5
0.641
27
13-9
51-4
0.270
6
34-3
61
0.562
33
7-7
39-5
0.195
n. 8
29.9
59-6
O.5OO
40
4.2
37.6
O.II2
13
28
58-1
0.482
47
2.4
31.2
0.077
IS
25-9
56.8
0.456
55
0.6
19.3
0.031
19
21
55-2
0.381
60
0
12.3
0
W = milligrams ozone dissolved per liter water. G = milligrams ozone in
one liter of the gas phase above the solutions. R = ratio of the dissolved to
undissolved ozone (W -J- G).
OZONE 474
The experiments of Schone (see preceding page) were repeated by Inglis
(1903). "The results confirm Schone's experiments and indicate that ozone,
when passed through water, is partly decomposed."
According to Moufang (1911) the solubility of ozone in distilled water ranges
from about 10 milligrams per liter at 2° to about 1.5 milligrams per liter at 28°.
The solubility is greatly affected by other substances in solution. Small amounts
of acids increase the solubility and render the aqueous solution of the ozone more
permanent. Alkalis decrease the solubility. Neutral salts (i.e., calcium sulfate)
increase the solubility.
SOLUBILITY OF OZONE IN DILUTE SULFURIC ACID.
(Rothmund, 1912.)
The explanation of the discrepancies concerning the solubility of ozone in water is
that the ozone quickly decomposes as the saturation point is reached. Rothmund,
therefore, determined the solubility in dilute HaSC^ in which decomposition takes
place much more slowly than in pure water. At o° the absorption coef. /3 (Bun-
sen, see p. 227) in o.i n H2SO4, is 0.487. The coef. remains practically the same
when the concentration of the ozone is changed over a wide range, hence Henry's
Law holds for ozone. The dissolved ozone has the same molecular weight as the
gaseous. The solubility depression which ozone experiences through o.i n
H2SO4 is calculated as 1.5%. Therefore, by extrapolation, it is calculated that
the abs. coef. ft of ozone in H2O at o°, is 0.494.
PALLADIUM CHLORIDE PdCl2.
When i gm. of palladium, as chloride, is dissolved in 100 cc. of H2O and shaken
with 100 cc. of ether, 0.02 per cent of the metal enters the ethereal layer at ord.
temp. When aq. 10% HC1 is used/p.oi per cent of the metal enters the ethereal
layer. (Mylius, 1911.)
100 cc. anhydrous hydrazine dissolve i gm. PdCl2, with evolution of gas and
formation of a black precipitate, at room temperature. (Welsh and Broderson, 1915.)
PALMITIC ACID CH3(CH2)14COOH.
SOLUBILITY IN AQ. AND ABSOLUTE ETHYL ALCOHOL.
i (Falciola, 1910.)
Cms. CH3(CH2)i4COOH per 100 cc.:
Absolute Aq. 75%
Alcohol. Alcohol.
10 2.8 0.24 0.05
20 9.2 0.43 0.08
30 ... 1.19 0.12
40 31.9 3-59 0-31
100 cc. sat. solution of palmitic acid in methyl alcohol of 94.4 vol. % (d =
0.8183) contain 1.03 to 1.17 gms. at 0.2°, equilibrium being approached from above.
The mixtures were simply allowed to stand in an ice chest for from 12 to 156
hours. (Hehner and Mitchell, 1897.)
SOLUBILITY OF PALMITIC ACID IN SEVERAL ALCOHOLS.
(Timofeiew, 1894.)
(
Alcohol.
Methyl Alcohol
it
d
Ethyl Alcohol
u
One hundred gms. of aq. 5% solution of bile salts dissolve about o.i gm. palmitic
acid. 100 gms. aq. 5% solution of bile salts containing i % of lecithin dissolve 0.6
gms1. palmitic acid. (Moore, Wilson and Hutchinson, 1909.)
Gms.
Gms.
to CH3(CH2)14COOH A,_,_i
to CH3(CH2)i4COOH
per 100 Gms.
i> .
per loo Gms.
Sat. Sol.
Sat. Sol.
'0
0.72
Propyl Alcohol
0
2.92
21
5-i
it
21
13.8
36
29-5
Isobutyl Alcohol
0
2.2
O
2
a
21
12.8
21
10. I
475
PALMITIC ACID
Cms. Stearic Acid
t°of
Gms. Stearic Acid
per 100 Gms.
Mixture.
Solidi-
fication.
per loo Gms.
Mixture.
100
57-2
55
90
56.42
5o
80
56.38
45
70
56.11
40
60
55-62
36
t°of Gms. Stearic Acid
Solidi- per 100 Gms.
fication. Mixture.
54.85 Eutec.
55-46
56.53
59-3i
62.62
30
25
20
10
O
SOLIDIFICATION POINTS OF MIXTURES OF PALMITIC AND STEARIC ACIDS.
(De Visser, 1898.)
Fifty gram samples of each mixture were used and great care taken to insure
accuracy of the determinations.
t°of
Solidi-
fication.
69.32
67.02
64-51
61.73
58.76
Additional determinations on this system by Dubowitz (1911) are, for the
most part, in good agreement with the above. According to Carlinfanti and
Levi Malvano (1909), however, the eutectic could^not be located and there were
indications of the existence of solid solutions.
DATA ARE GIVEN FOR THE SOLIDIFICATION POINTS OF THE FOLLOWING
MIXTURES:
Palmit c Acid + Tripalmitin
-|- + Stearic Acid.
4- 4- Tristearin.
+ Tristearin + Stearic Acid.
+ Tristearin.
Tripalmitin + Tristearin -f Stearic Acid.
-j- Stearic Acid.
Palmitic Acid Cetyl Ester + Paraffin.
(Kremann and Klein, 1913.)
(Kremann and Kropsch, 1914.)
(Kremann and Klein, 1913.)
(Palazzo and Battelli, 1883.)
PAPAVEBINE C20H21N04.
IOO gms. carbon tetrachloride dissolve 0.203 gm. at 17°. (Schindelmeiser, 1901.)
100 gms. carbon tetrachloride dissolve 0.518 gm. at 20°. (Gori, 1913.)
loo gms. ethyl ether dissolve 0.38 gm. at 10°.
100 gms. of each of the following solvents dissolve the stated amount of papaver-
ine at 20°. Aniline, 29 gms.; pyridine, 8 gms.; piperidine, I gm.; diethylamine,
0.4 gm. (Scholtz, 1912.)
PARAFFIN.
.SOLUBILITY OF OZOKERITE PARAFFIN OF MELTING POINT 64°-65° AND
SP. GR. AT 20° = 0.917 IN SEVERAL SOLVENTS AT 20°.
(Pawlewski and^Filemonowicz, 1888.)
Gms. Paraffin per 100
Gms. Paraffin per 100
Solvent.
Carbon Bisulfide
Benzine, boiling below 75°
Turpentine, b. pt. i58°-i66°
Cumol, com. b. pt. 160°
" frac. iso°-i6o°
Xylene, com. b. pt. i35°-i43°
" frac. i35°-i38°
Toluene, com. b. pt. io8°-no
frac. io8°-io9°
Chloroform
Benzene
Ethyl Ether
Isobutyl Alcohol, com.
F.-pt. data for paraffin + stearin are given by Palazzo and Battelli (1883).
Gms.
cc.
Solvent.
Gms.
cc.
Solvent.
Solvent.
Solvent.
Solvent.
12.99
Acetone
0.262
0
.209
n-73
8
'.48
Ethyl Acetate
0.238
. . .
6.06
5
.21
" Alcohol
0.219
4. 26
3
.72
Amyl Alcohol
O.2O2
0
.164
3-99
3
•39
Propionic Acid
0.165
. . .
3-95
3
•43
Propyl Alcohol
o. 141
4-39
3
•77
Methyl Alcohol
O.O7I
o
.056
3 3-88
3
•34
Methyl Formate
0.060
3-92
3
.41
Acetic Acid
0.060
0
.063
2.42
3
.61
" Anhydride
0.025
1.99
1
•75
Formic Acid
0.013
0
.015
i-95
Ethyl Alcohol 75%
0.0003
0.285
o
.'228
PENTANE
476
Isopentane Rich
Layer.
Phenol Rich
Layer.
4-5
87
7
83-5
"•5
80
18
75-S
29-5
68
40
58
PENTANE CH3(CH2)3CH8.
Data for the solubility of pentane in liquid carbon dioxide, determined by the
synthetic method, are given by Biichner (1906).
IsoPENTANE (CH3)2CH.CH2CH3.
RECIPROCAL SOLUBILITY OF ISOPENTANE AND PHENOL. (Campetti and Del Grosso, 1913.)
Gms. Phenol per 100 Cms.
20
30
40
50
60
65
66 crit. temp. 50
F.-pt. data for mixtures of hexachloro-a-keto 7--R-pentene, C5C16O, +penta
chloromonobromo ex-keto y-R pentene, C5Cl6BrO, are given by Kiister (1890, 1891).
PEPTONE.
100 gins. H2O dissolve 42.2 gms. peptone at 20-25°. (Dehn, 1917.)
" pyridine " 0.22 " "
aq. 50% pyridine " 12.6 "
PERCHLORIC ACID HC1O4.
SOLUBILITY IN WATER, (van Wyk, 1902, 1905.)
Mixtures of HC1O4 and water were cooled until crystals appeared and then very
gradually warmed and constantly stirred while an observation was made of the
exact temperature at which the last crystal disappeared. At certain concentrations
and temperatures unstable solid phases were obtained, also, curves for two series of
mix crystals were encountered. The methods for detecting these phases consisted
in seeding the saturated solutions with the several different crystalline forms, and
observing the change in rate of cooling during the solidification of the mixture.
The data for the mix-crystal curves I and II are not given in the following table:
Mols. HC1O4
t°. per 100 Mols. Solid Phase. t°.
HC1O4+H2O.
Mols. HC104
per 100 Mols. Solid Phase.
HC104+H2O.
0
0
Ice -32
26
HC104.2*H20
— 10
5
-29
.8
28
•57
— 21
7
-44
27
HC104.2H2O
-34
•5
9
-41
27
.25 «'
-54
ii
-34
28
ii
-50
•5
19
HC104.3iHjO — 24
29
•9
-45
20
-17
.8m.
^•33-3
-42
•3
21
— 21
•5
36
"
-41
•4
22.22
-23
.6
36
.5 " +HClO4.HaO
-43
23-5
— 12
•5
37
HC104.H2O
-40
•5
22.5
HC104.3H2Oa 1+3
38
-39
•5
22.75
28
40
.8
-37
.6
24
40
43
•7
-37
•5
26
« 50 m. pt
50
-38
.8
27
45
59
•9
-47-8
22.5
HC104.3H2O/3 27
•5
71
•5
-44
24
17
77
.2
-43
•5
24-5
+ 2
.2
83
•3
-43
.2
25
" —21
•5
90
•7
-44
•5
26
-40
94
-37
.2
25
HClO4.3H2Oa+HC104.2|H2O — IO2
ICO
477 PETROLEUM ETHER
PETROLEUM ETHER.
100 cc. H2O dissolve 0.005 cc. petroleum ether at 15°. (Groschuff. 1910.)
PHENACETIN (p Acetphenetidin) CeH^OC^NHCHaCO p. •
SOLUBILITY IN AQUEOUS ALCOHOL AT 25°.
(Seidell, unpublished.)
Wt. % C2H5OH
in Solvent. __
, f Cms. C6H4(OQH5)
9 t c£l NHCH3CO per 100
j Sat. Sol. Gms. Sat. Solution.
Wt. % OH5OH
in Solvent.
Sa«,
Cms. Sat. Solution.
o (water)
I
0.0766
70
0.879
6.25
10
0.984
0.14
80
0.858
7.63
20
0.968
0.28
85
0.847
7.88
30
0.952
0.65
90
0.834
7.82
40
0-935
1-50
92-3
0.827
7.70
50
0.917
2.85
95
0.821
7-45
60
0.898
4-55
100
0.806
6.64
loo gms. H2O dissolve 1.43 gms. phenacetin at "the b. pt. (U.S. P., VIII.)
ioogms-92.3 wt. % alcohol dissolve about^o gms. phenacetin at the b. pt. "
SOLUBILITY OF PHENACETIN IN SEVERAL SOLVENTS.
(Seidell, 1907.)
Gms. Phenacetin Gms. Phenacetin
Solvent. t°. per 100 Gms. Solvent. t°. per 100 Gms.
Sat. Solution. Sat. Solution.
Acetone 3°~3I 10.68 Benzene 30-31 0.65 (0.873)
Amyl Acetate 3°~~3I 2.42 (0.865) Chloroform 25 4.76
Amyl Alcohol 25 3.51 (0.819) Ether 25 1.56
Acetic Acid (99.5%) 21.5 13.65 (1.064) Toluene 25 0.30 (0.863)
Aniline 3°~3I 9-46 (1.025) Xylene 32.5 1.25 (0.847)
Benzaldehyde 3°~3I 8.44 (1.063)
(Figures in parentheses are Sp. Gr. of Sat. Solutions.)
100 cc. petroleum ether dissolve 0.015 gm. phenacetin at room temp. (Salkower, 1916.)
100 gms. pyridine dissolve 17.39 gms. phenacetin at 20-25°. (Dehn.igi?.)
100 gms. aq. 50% pyridine dissolve 28.94 £m$' phenacetin_at 20-25°. "
PHENANTHRAQUINONE
SOLUBILITY IN BENZENE AND IN ETHYL ACETATE.
(Tyrer, 1910.)
Solubility in Benzene. Solubility in Ethyl Acetate.
,„ Sp Gr.of Gms' (CaHMOW. s Gr of Gms.
*° SatPSolution. -- *° SatPSolution.
10 0.8902 0.412 10 0.9102 0.518
15 0.8850 0.471 2O 0.9025 0.626
20 0.8800 0.538 30 0.8906 0.770
30 0.8698 0.738 40 0.8789 0.995
40 0.8601 1-032 50 0.8674 1.292
50 0.8506 x-354 60 0.8561 1.640
60 0.8415 1.760 65 0.8508 1.902
70 0.8327 2.687 7° 0-^454 2.215
80 0.8241 3.770 75 0.8401 2.515
NOTE. — The Sp. Gr. determinations given in the above table and in the tables
for anthracene and anthraquinone, pp. 81 and 82, are not included in the original
paper of Tyrer (1910) but, in response to my request, have been kindly supplied
for the present volume. I am also indebted to Dr. Tyrer for the modified form
of his original tables showing the solubilities of anthraquinone and phenanthra-
quinone in mixed solvents. (A. S.)
PHENANTHRAQUINONE
478
SOLUBILITY OF PHENANTHRAQUINONE IN MIXTURES OF ORGANIC SOLVENTS.
(Tyrer, 1910.)
In C6H6 + Hydrocarbons In CHC13 + Pentane In CH3COOC2H5 + Hydro-
(i) at 48°.
Per cent Gms
at 14.5°.
. Phenan- Per cent Gms. Phenan-
carbons(i) at 48°.
Per cent Gms. Phenan-
Mixe^
Solvent
thraquinone CHC13 in thraquinone CH3COOC2H5 thraquinone
per loo Gms. Mixed per 100 Gms. in Mixed per 100 Gms.
Solvent. Solvent. Solvent. Solvent. Solvent.
0
0
.0708
0
0.
025
O
0
•073
10
0
.088
10
o.
045
14
.19
0
.126
20
o
.118
20
0.
080
27
•37
O
.207
30
0
.160
30
0.
"5
39
•94
0
•335
40
0
.228
40
0.
165
52
.12
0
•494
50
o
.318
50
0.
220
63
-56
0
-656
60
0
.440
60
0.
330
74
.19
O
.817
70
0
.588
70
0.
525
84
.62
0
•993
80
0
•772
80
o.
805
90
I
•073
90
I
.004
90
I.
415
IOO
I
• 230
IOO
I
.288
IOO
2.
402
(O
Distilled from petroleum, b. pt. - 82'
'-92
°. (See note, preceding page.)
PHENANTHRENE Ci4Hi0.
SOLUBILITY IN
ALCOHOL
AND IN TOLUENE
.*
(Speyers
— Am.J.Sci.[
4] 14, 295, 'oa.)
In Alcohol.
In Toluene.
Gms. CwHro per
Sp. Gr. of
Gms. Ci4Hio per
Sp. Gr. of
t
loo Grams
Solutions
loo G
rams
Solutions
CjzHjiOH. CHzO at 4°-)
QHfi.CHa
(H20 at 4°
.)
0
3-65
0.814
23
.0
0.925
10
3-80
0.807
30
.O
0.929
20
4.6
0.801
42
• O
Q-934
25
5-5
o-7P9
50
.O
0-939
30
6.4
0-797
58.0
0-943
40
8.2
o-795
76
.0
o-955
50
10.6
o.794
95
.0
0.971
60
15.6
o-797
"5
.0
0.989
70
0.815
.0
1.007
80
0.865 (76
-4°) 155-0
1.027
• Calculated from the original results which are given in terms of gram molecules of Phenanthrene
per loo gram molecules of solvent, and for irregular intervals of temperature.
Behrend, 1892, reports 2.77 gms. phenanthrene per 100 gms. alcohol at 12.3°,
and 3.09 gms. at 14.8°.
SOLUBILITY OF PHENANTHRENE IN ORGANIC ACIDS. (Timofeiew, 1894.)
Gms. Ci4H10 Gms. CUH10
Acid. t°. per 100 Gms. Acid. .! t°. per 100 Gms.
Sat. Sol. Sat. Sol.
Acetic Acid 23 8.31 Propionic Acid
9.8
Butyric Acid
23
39
70
23
39
34-6
15-6
21
23
39
62.
23
17
21.4
40.3
12.3
16.6
(Aschan, 1913.)
Isobutyric Acid
Valeric Acid
100 gms. 95% formic acid dissolve 0.46 gms. CuHio at 20.8
F.-pt. data for mixtures of phenanthrene and each of the following compounds
are given by Kremann et. al., (1908); 1.2.6 dinitrotoluene, 1.2.4. dinitrotoluene,
1.3.4 dinitrotoluene, trinitrotoluene and trinitrobenzene. Results for mixtures
of phenanthrene and 2.4 dinitrotoluene are given by Kremann and Hofmeier
(1910).
479
PHENANTHRENE
SOLUBILITY OF PHENANTHRENE IN SEVERAL SOLVENTS AT 25°.
(Hildebrand, Ellefson and Beebe, 1917.)
Solvent.
Alcohol
Benzene
Carbon Bisulfide
Cms. CuHjo per 100
Gms. Solvent.
4.91
59-5
80.3
Solvent.
Carbon Tetrachloride
Ether
Hexane
Gms. CuHjo per too
Gms. Solvent.
26.3
42.9
9-15
SOLUBILITY OF PHENANTHRENE PICRATE IN ABSOLUTE ALCOHOL.
(Behrend, 1892.)
Grams per 100 Grams Saturated Solution.
Picric Acid + Phenanthrene •= Phenanthrene titrate.
12-3 0.91 O.yi 1.62
14.3 i .00 0.78 1.78
17.5 1.05 0.82 1.87
SOLUBILITY OF PHENANTHRENE PICRATE IN ALCOHOLIC SOLUTIONS
CONTAINING PICRK; ACID AND ALSO PHENANTHRENE.
(Behrend.)
Grams Added to 62 cc. Abs. Alcohol. Gms. per 100 Gms. Sat. Solution.
to. , - » - N r.
P. Picrate + Picric Ac. + Phenanthrene. Pi
12.3
12-3
12 -S
12-3
17-5
17-5
17-5
17-5
17-5
PHENOL C6H5OH.
SOLUBILITY IN WATER.
(Alexejew, 1886; Schreinemaker, 1900; Rothmund, 1898.)
The determinations were made by the "Synthetic Method," for which,
Note, p. 1 6.
Gms. Phenol per 100 Gms.
\ Picrate + Picric Ac. + Phenanthrene
1-4
0
o-5
1.4
0.8
o
0
0.9
2.1
0.8
0
4.0
•4
O.I
0
•4
O.2
0
•4
1.0
0
•4
4.0
o
•4
o.o
2.2
Picric Ac.
+ Phenanthrene *-
P. Picrate
0-534
I-4I3
1-947
0.409
2.I4I
2-550
o-354
2-77
3.124
0.139
5.626
c . 76?
I-I59
o-75
I • Q I
1.285
0.68
1-97
2-45
o-37
2.82
6.15
0.195
6-345
0.423
3.276
3-699
i> .
Aqueous Layer.
Phenol Layer.
10
7-5
75
20
8-3
72.1
30
8.8
69.8
40
9.6
66.9
50
12
62.7
55
I4.I
59-5
60
I6.7
55-4
65
21-9
49.2
68.3 (crit. temp.)
33-4
Results confirming the above, and also viscosity measurements, are given by
Scarpa (1904).
The complete T — x data for the system are given by Smits and Maarse (1911).
F.-pt. data for the system are given by Rozsa (1911) and Paterno and Ampola
Vaubel (1895) states that ipo gms. sat. aqueous solution contain 6.1 gms.
phenol at 20°. Sp. Gr. of solution = 1.0057.
PHENOL
480
PHENOL.
SOLUBILITY OF PHENOL IN AQUEOUS ACETONE SOLUTIONS.
(Schreinemakers, 1900.)
In 4.24%
Acetone.
Grams Phenol per
In 12.2%
Acetone.
Gms. Phenol per
In 24.6%
Acetone.
Gms. Phenol per
In 59-9%
Acetone.
Gms. Phenol per
A0 100 Gms.
100 Gms.
100 Gms.
100 Gms.
Aq. Acetone
Layer.
Phenol
Layer.
Aq . Acetone
Layer.
Phenol *
Layer.
Aq. Acetone
Layer.
Phenol '
Layer.
Aq . Acetone Phenol
Layer. Layer
20
...
. . .
26. o 60. 5
3°
S-o
74.0
4.0
71.0
6.0
69.5
28.5 57.0
40
5-5
70.0
32.0 52.0
5°
5-7
67.0
5-0
67.0
8.0
64.0
34- 5§ 49- °§
60
6-5
61.0
36.51! 46. 5 U
70
9.0
51.0
7-5
57-5
19.0
57- °
(49-5°) 41-5
80
14. o
34-0
10.5
49-5
14.0
52-5
(84°) 22.5
20. 4*
23. ot
47. ot
(90.3°) 25.
o
26. 5t
44. o t
(90. 5°) 35-
, o
•90°
t8S°
t87°.S
§45°
!!47°.5
The figures in the above table were read from curves plotted from the original
results. Similar data are also given for acetone solutions of seven other concen-
trations.
The determinations were made by adding various quantities of phenol to the
mixtures of water and acetone and observing the temperature at which the two
layers became homogeneous. The isothermal lines for 30°, 50°, 68°, 80°, 85° and
87° were located. The results for 30° and 80° are as follows: (Schreinemakers, 1900.)
Results at 30°.
Gms. per 100 Gms. Mixture. Gms. per 100 Gms. Mixture.
Results at 80°.
Gms. per 100 Gms. Mixture.
H20.
(CH^CO.
C6H6OH.
H20.
(CH3)2CO.
C6H6OH.
H20.
(CHs),CO.
C6H5OH.
92
0
8
18.4
34-i
47-5
83.3
3-7
13
92-3
i-7
6
17.2
25-8
57
82.9
7-i
10
91
4
5
17.9
81.1
64
74-7
13-8
"•5
88.4
7.6
4
19.1
12.9
68
61.8
20.2
18
81
IS
4
21 .1
9-9
69
52-5
24-5
23
70.9
23.1
6
22.6
7-4
70
40.6
27.4
32
62.1
28.9
9
25.2
4.6
70.2
32.2
21.8
46
51.6
34-9
13-5
27.1
2-3
70.6
33-4
15-6
5i
39-8
40.2
20
28.7
i-3
70
35-4
ii. 6
53
28.9
43-i
28
30
o-5
69-5
40-5
7-5
S2
21.8
40.2
38
49-7
4-3
46
62.7
2.8
34-5
SOLUBILITY OF PHENOL IN BENZENE AND IN PARAFFIN,
(Schweissinger, 1884-85.)
Gms. C6H5OH per 100 Gms. Solvent at:
Solvent.
Paraffin
Benzene
16°.
1.66
2-5
8-33
10
43".
5
IOO
Data for equilibrium in systems composed of phenol, water and each of the fol-
lowing compounds are given by Timmermans (1907): NaCl, KC1, KBr, KNO3,
, MgSO4, tartaric acid, salicylic acid, succinic acid and sodium oleate.
48 1
PHENOL
MISCIBILITY OF AQUEOUS ALKALINE SOLUTIONS OF PHENOL WITH SEVERAL
ORGANIC COMPOUNDS INSOLUBLE IN WATER.
(Scheuble, 1907.)
To 5 cc. portions of aq. KOH solution (250 gms. per liter) were added the given
amounts of the aq. insoluble compound from a buret and then the phenol, drop-
wise, until solution occurred. Temperature not stated.
Composition of Homogeneous Solutions.
cc. Aq. KOH.
5
5
5
5
5
cc. Aq. Insol. Cmpd. Gms. Phenol.
2 (= 1.64 gms.) Octyl * Alcohol 2.6
5 (= 4.1 gms.) 3.9
2 (= 1.74 gms.) Toluene 4.9
3 (= 2.61 gms.) Toluene 6.7
2 (== 1.36 gms.) Heptane 15
1 = the normal secondary octyl alcohol, i. e., the so-called capryl alcohol, CH3(CH2)s.CH(OH)CHj.
SOLUBILITY OF PHENOL IN AQUEOUS SOLUTIONS OF DEXTRO TARTARIC
ACID AND OF RACEMIC ACID.
(Schreinemakers, 1900.)
In 5.093% Acid. In 19.34% Acid. In 40.9% Acid.
Gms. Phenol per 100 Gms. Gms. Phenol per 100 Gms. Gms. Phenol per too Gms
30
50
60
65
67-5
69*
Aq. Acid
Layer.
7-5
14-5
19-5
25
Phenol
Layer.
72.5
65.5
58
53
48.5
t°. '
Aq. Acid Phenol
Layer. Layer.
50
10 77
60
12.5 72
70
19 64
75
29 56
77*
47
47-5
70
80
85
90
95<
97"
Aq. Acid.
Layer.
13
16.5
2O
26.5
39
Phenol
Layer.
77
74
63-5
54
* Critical temperature.
Identical results were obtained with the dextro and racemic acids, showing that
both have exactly the same influence on the formation of layers in the system
water-phenol.
DISTRIBUTION OF PHENOL BETWEEN:
AMYL ALCOHOL AND WATER AT 25°. BENZENE AND WATER AT 2o°r
(Herz and Fischer — Ber. 37, 4747, '04.) (Vaubel — J. pr. Ch. [2] 67, 4?6, 'op
Millimols Phenol
per 10 cc.
Gms. Phenol
per 100 cc.
Alcoholic Aqueous
Layer. Layer.
0- 75 0-P47
0.9 0.05
I.I 0.07
e. 6 o. 16
54-1 3-83
56-3 3-9
Alcoholic Aqueous
Layer. Layer.
o. 705 o. 0441
o. 846 o. 047
1.035 0.066
2.445 0.150
50.88 3.601
52.93 3.667
Gms. Phenol in1
Volumes of Solvents
i Gm. Phenol ^5" .
Layer. Layer
5occ.H2O+ 5occ.C6H8 0.286 0.714
" -r-ioocc. " o. 1188 0.8212
" +151000. u 0.0893 0.9107
" *f20occ. " 0.0893 0.9107
DISTRIBUTION OF PHENOL BETWEEN WATER AND BENZENE AT 20°.
(Philip and Bramley, 1915.)
Gms. Phenol per Liter. *
Ratio - •
a
2.194
2.189
2.184
2.176
2.181
Results are also given for the effect of NaCl, KC1 and of LiCl upon the above
distribution.
Aq. Layer, a.
C6H6 Layer, b.
0-945
2.073
0.888
1.944
0.711
1-553
0-594
0-475
1.293
i 036
lims. .Fnei
iol per Liter.
A. ....
Ratio-.
a
2.173
2.175
2.180
2.189
Aq. Layer, a.
0-356
0.238
O.II9
0.0601
QH6 Layer; b.
0.7736
o.5J77
0.2594
O.I3I4
PHENOL
482
DISTRIBUTION OF PHENOL BETWEEN WATER AND BENZENE AND
BETWEEN AQUEOUS K2SO4 SOLUTIONS AND BENZENE AT 25°.
(Rothmund and Wilsmore — Z. physik. Ch. 40, 623, '02.)
NOTE. — The original results, which are given in terms of gram
jnols. per liter, were calculated to grams per liter, and plotted on cross-
section paper. The following figures were read from the curves
obtained.
Between H2O and C6H«.
Effect of K2SO4 upon the Distribution.
Grams C8H5OH
per Liter of:
Gms. K2SO4
per Liter
(i) Gms. CeH6OH
per Liter of:
GOGms. C6H5OH
per Liter of:
fi20
Layer.
Layer.
Aq.
Solution.
Aq.
Layer.
QjH,,
Layer.
Aq.
Layer.
Layer.
5
10
L36
17.08
59-96
9-52
26.28
10
28
2.72
16.92
60.63
9-50
26.38
20
e
5-44
10.89
16.85
16-44
60.92
62.73
9.46
9-35
26.55
27.06
C5
128
21.79
15.89
65.19
9.09
28.27
30
200
43-59
14-85
69.71
8.68
30.21
35
300
87.18
12.92
78.00
r-79
34.38
40
410
45
520
So
610
(i) First series.
(2)
Second series.
EQUILIBRIUM IN THE SYSTEM PHENOL, BENZENE AND WATER AT 25°.
(Horiba, 1914-1916.)
Cms. per 100 Cms. Sat. Sol.
Solid Phase.
Q,H6OH
C«H6OH.
C6H6.
H20.
81.06
18.94
0
89.78
7-92
2.30
92.31
4.07
3.62
95-14
o
4.86
The results for the conjugated liquid layers are as follows:
Upper Layer.
Cms. per 100 Gms. of the Liquid.
Lower Layer.
Gms. per 100 Gms. of the Liquid.
QHjOH.
C6H,.
H20.
C6H6OH.
CeHs.
H2O.
0
99-95
0.05
O
0.198
99 . 802
4-78
94-98
O.24
i-43
0.21
98.36
17.36
81.83
0.81
2.80
O.2I
96.99
21.15
77.22
1.63
3.01
O.2I
96.77
28.01
69.81
2.18
3-35
0.21
96.44
44-39
50-56
5-05
4.07
O.I9
95-74
55-8o
36-13
8.07
4-58
0.19
59-23
74-5
3
22.5
5-65
0.17
94.18
70.70
0
29.29
8.195
0
91-805
Data for this system are also given by Rozsa (1911).
The coefficient of distribution of phenol between olive oil and water at 25°,
cone, in oil -*- cone, in H2O, is given by Boeseken and Waterman (1911) as greater
than 9 and less than 10.3. The figure was obtained by dividing the solubility of
phenol in olive oil by the solubility in water, each being determined separately.
Results for this system are also given by Reichel (1909).
According to Greenish and Smith (1903), 100 cc. of olive oil dissolve about 50
gms. of phenol at 15.5°. These authors report that 100 cc. of glycerol dissolve
about 300 gms. of phenol at 15.5°.
PHENOL
DISTRIBUTION OF PHENOL BETWEEN WATER AND CARBON TETRA
CHLORIDE AT 20°.
(Vaubel — J. pr. Ch. [2] 67, 4?6, '03.)
Grams Phenol in:
Volumes of Solvents.
Gms. Phenol
Used.
50 cc. H2O+ 10 cc. CC14
" ' + 20 CC.
+ 30 cc.
+ 50 cc.
+ 100 CC.
" + 1500:.
" +200 CC.
H2O Layer.
CCU Layer.
0.8605
0.1285
0.7990
O.I9OO
0.7275
0.2615
0-6435
Q-3455
0.4680
0.5210
0.3645
0.6245
0.3240
0-6650
DISTRIBUTION OF PHENOL BETWEEN WATER AND ORGANIC SOLVENTS AT 25°.
(Herz and Rathmann, 1913-)
Results for:
H2O and Tetrachlor
Ethane.
Mols. C6H5OH per Liter.
H,0 -d Chloroform.
Mols. C6H6OH per Liter.
Mols. C6H5OH per Liter.
H2O Layer. CHC13 Layer.
0-0737 0.254
0.163 0.761
O.2II 1.27
0.330 3-36
0.436 5-43
H2O and Pentachlor
Ethane.
Mols. C6H5OH per Liter.
H2O Layer. CC14 Layer.
0.0605 0.0247
O.I4O 0.072;
0.213 O.I4I
o-355 o-392
0.489 1.47
0.525 2.49
H2O and Trichlor
Ethylene.
Mols. C6H5OH per Liter.
H2O Layer. C2H2 C14 Layer.
0.023 0.061
0.0345 0.094
O.oSl 0.265
O.II4 0.406
0.151 O.6l7
0.155 0.651
H2O and Tetrachlor
Ethylene.
Mols. C6H5OH per Liter.
H2O Layer. C2HC16 Layer.
o . 0420 o . 0495
0.0866 o.no
0.150 0.226
O.222 0.432
O.28O 0.708
0.333 I-I7o
H20 Layer. CHC1:CC12 Layer.
o . 044 o . 046
o.ioi 0.107
0.180 0.236
0.236 0.388
0-277 0.555
0.339 0-986
H20 Layer. CC12:CC12 Layer.
0.0653 0.0277
0.143 0.0650
0.327 0.198
0.421 0.4II
o . 490 o . 684
DISTRIBUTION OF PHENOL AT 25° BETWEEN:
(Herz and Fischer — Ber. 38, 1143, '05.)
Water and m Xylene.
Water and Toluene.
Millimols C6H6OH
Grams C6H6OH
per
10 CC.
per 100
cc.
CflHgCH;
Layer.
j H20
Layer.
C6H5CH3
Layer.
H26
Layer.
1.244
0.724
1.169
0.681
3-047
1.469
2.865
1.381
4.667
2 .200
4-389
2.068
6.446
2.861
6.o6l
2.691
14.960
4-750
14.07
4.467
I7-725
5-346
16.69
5.027
47-003
7.706
44-20
7.246
8.087
50.58
7.604
90.287
9.651
84.89
9.074
Millimols
per 10 cc
mC6H4(CH3)2
Layer.
1.610
4.787
I2.2IO
22.7l8
34.827
51.352
77.703
H20 '
Layer.
1.071
2.726
5.l68
6.994
8.124
9.123
10.050
Grams C6H6OH
per zoo cc.
H2O'
Layer.
Layer.
I.5I4
4.501
11.22
21.36
32.75
48.28
73-07
1.007
2.563
4-86(5
6-57?
7.640
8.578
9-45<
PHENOL 484
FREEZING-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR
MIXTURES OF PHENOL AND EACH OF THE FOLLOWING COMPOUNDS:
Dimethylpyrone. (Kendall, igua.) Bromotoluene. (Paterno and Ampola, 1897.;
Phenylhydrazine. (Cuisa and Bernardi, 1910.) 0 Toluidine. (Kremann, 1906.)
Picric Acid. (Philip, 1903; Kremann, 1904.) p Toluidine. (Kremann, 1906; Philip, 1903.)
Picric Acid +Other Cm'p'ds. (Kremann, '04.) Urea (Kremann & Rodenis, 1906; Philip, 1903.)
Pyridine. (Bramley, 1916; Hatcher &Skirrow, 1917.) Methyl Urea. (Kremann, 1910.)
Quinoline. (Bramley, 1916.) as Dimethyl Urea.
Resorcinol. (Jaeger, 1907.) s Dimethyl Urea.
Sulfuric Acid. (Kendall and Carpenter, 1914.) Urethan. (Mascarelli & Pestalozza, 1908, 1909.)
Thymol. (Paterno and Ampola, 1897.) p Xylene. (Paterno and Ampola, 1897.)
m Xylidene. (Kremann, 1906.)
PHENOLATE of Phenyl Ammonium.
SOLUBILITY IN WATER.
(Alexejew, 1886.)
The determinations were made by the synthetic method (see p. 16). The re-
sults were plotted and the following figures read from the curve:
Gms. Phenolate per 100 Gms. Gms. Phenolate per 100 Gms.
t°. t *- <k t°. t * N
Aq. Layer. Phenolate Layer. Aq. Layer. Phenolate Layer.
10 3 94 no 9 76
30 4 93 120 12 69
50 5 91 130 17.5 60
70 6 87.5 140 crit. temp. 40
90 7 83
AminoPHENOLS. See last line p. 138.
5 TribromoPHENOL C6H2Br3OH. .
Data for the solubility of mixtures of symmetrical tribromophenol and symmetri-
cal trichlorophenol in diluted methyl alcohol at 25° are given by Kiister and Wiirfel
(1904-05). The results are presented in terms which are not clearly explained.
SOLUBILITY OF MIXTURES OF 5 TRIBROMO PHENOL AND 5 TRICHLORO PHENOL
IN METHYL ALCOHOL AT 25°.
(Thiel, 1903; from Wiirfel, 1896.)
Molecular per cent CeH2.OH.Bra n Solubility of
' In Solid. In Solution. " C«H2.OH.a3. C6H2.OH.Br3'.
o o 0.204 o 0.204
4.49 3-59 0.194 0.007 0.201
10.13 7 -58 0.191 0.016 0.206
16.28 12.15 0.172 0.024 0.196
62.44 13.07 0.204 0.031 0.235
69.88 15-86 0.150 0.028 0.178
81.76 19.01 0.096 0.023 0-118
84.66 24.05 0.069 O.O22 O.O9I
87-53 32-46 0.043 0.021 0.063
93.62 47*87 O-O2I O.OI9 O.O4O
loo. o loo. o o-o 0.019 0.019
NitroPHENOLS C6H4(OH)NO2 o, m and p.
100 gms. sat. solution in water contain 0.208 gm. o nitrophenol at 20°.
" 2.14 gms. m
1.32 p (Vaubel, 1895.)
F.-pt. data for mixtures of m nitrophenol and water and for p nitrophenol and
water are given by Bogojawlewsky, Winogradow, and Bogolubow (1906).
NitroPHENOLS
NitroPHENOLS C6H4(OH).NO2 o, m and p.
SOLUBILITY OF EACH SEPARATELY IN WATER.
Gms. per 100 Gms. Sat. Sol.
(Sidgwick, Spurrell and Davies, 1915.)
Gms. per too Gms. Sat. Sol.
Ortho.
Meta.
Para.
40
O
•330*
3-
02*
3-
28
100
50
* O
.388
3-
68
4-
22
no
60
o
•463
4-
54
5-
53
120
70
0
.560
5-
80
7-
50
120
80
o
.685
7;
90
10.
85
140
90
0
.856
II .
69
21.
2
150
92.8
crit. t. ,
, . .
. .
OC
>
160
98.7
crit. t.
CO ...
200+
Ortho. Meta. Para.
1.078
i-59
2-32
2 . 90
3-75
crit. t. oo
* in above table indicates that a solid phase is present.
The above determinations were made by the synthetic method. M. pt. of o =
44.9°; of m = 95.1°, of p = 113.8°. Triple pt. for o = 43.5° at cone. 99.48 and
0.35; for m = 41.5° at cone. 74 and 3.16; for p = 39.6° at cone. 71.2 and 3.26.
One liter sat. solution in water contains 3.89 gms. o nitrophenol at 48°.
One liter sat. solution in i.o n o C6H4(ONa)NO2 contains 9.6 gms. o nitrophenol
at 48°. (Sidgwick, 'io.)
SOLUBILITY OF o NITROPHENOL IN LIQUID CARBON DIOXIDE. (Buchner, 1905-6.)
Gms. o C,H4(OH)NO2
t°. per 100 Gms.
Sat. Sol.
-52
1.9
-40
2-5
— 20
3-8
0
+ 10
5-2
7-7
Gms.0C,H4(OH)NO2
per 100 Gms.
Sat. Sol.
12.5
14
15
16
20
io
21.2
33-8
48.5
60 . 7
100 gms. 95% formic acid dissolve"! 6.06 gms. 0C6H4(OH)NO2at 20.8°. (Aschan, '13.)
ioogms.95%formicaciddissolve23.44gms.£C6H4(OH)NO2at 18.6°.
One liter of sat. solution of the pale yellow form of p nitrophenol in benzene,
contains 7.1 gms. p C6H4(OH)NO2 at 5°, determined by the f.-pt. method.
(Sidgwick, 1915.)
SOLUBILITY OF THE THREE NITROPHENOLS, SEPARATELY, IN TOLUENE,
BROMOBENZENE AND IN ETHYLENE DIBROMIDE. (Sidgwick, Spurrell and Davies. 1915.)
f°
Gms. o C6H4(OH)NO2 per 100 Gms. Sat. Sol. Gms. p C6H4(OH)NO2 per 100 Gms.Sat. Sol.
l>
In
C6H5CH3. In C6H6Br,
, In C2H4Br2.
In C6H5CH3. In C6H6Br.
InC2H4Br2.
15
46.9
40
70
18
•5
. .
.
31
20
55-2 48-8
47
,8
80
28
.1
32
•7
52 \
25
64.6 57.7
56
.8
90
54
• 4
59
•7
73-2
30
74.6 67.2
67.
2
100
79
.6
80
.6
88.5
35
84-5 78.3
79
IIO
96
•3
96
•3
98
40
93.1 89.7
9°
6
t<
Gms. m C«H4(OH)NO2
per loo Gms. Sat. Sol.
Gms. m C6H4(OH)NO2
t°. per loo Gms. Sat. Sol. t°.
Gms. m C6H4(OH)NO,
per loo Gms. Sat. Sol.
in C6H5CH3.
in C,H6CH3.
in C6H6CH3.
.39
.6
4.63
64.8
16.44
78-5
70
•50
45
.8
6
67-7
2O.26
82.3
79
•57
48
•9
7-03
71-5
33-16
88.8
91
•43
54
9.II
74-5
46.93
95.1
IOO
58
11.28
75-7
57-71
DiNitro
PHENOL C6H6.
OH.(N02)2.
100 gms. abs. methyl alcohol dissolve 6.3 gms. C6H3.OH.(NO2)2 at 19.5°.
100 gms. abs. ethyl alcohol dissolve 3.9 gms. C6H3.OH.(NO2)2at 19. 5°. (deBruyn, '92.)
PHENOLS
486
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES CONTAINING SUBSTITUTED PHENOLS.
o Bromophenol + p Bromophenol.
o Chlorophenol 4- P Chlorophenol.
o lodophenol + p lodophenol.
5 Tribromophenol + s Trichlorophenol.
2.4.6 Tribromophenol + Acetyl tribromophenol.
o Chlorophenol + Quinoline.
+ Pyridine.
o Nitrophenol + Acetyl o Nitrophenol.
o Nitrophenol + a Dinitrophenol.
+ p Toluidine.
p Nitrophenol + p Nitrosophenol.
Each of o, m and p Nitrophenol + Dimethylpyrone.
+ Picric Acid.
+ Sulfuric Acid.
+ Urea.
2.4 Dinitrophenol + Dimethylpyrone.
PHENOLPHTHALEIN (Ce^OH^CO.CeKUCO.
loogms. H2O dissolve 0.0175 gm. phenol phthalein at 20°.
(Acree and Slagle, 1909.)
0.04 at 20-25°. (Dehn.'i?.)
" Pyridine " 796. gms.
" aq. 50% pyridine " 300
PHENYL ALANINE « C6H6NHCH(CH3)COOH.
Data for the solubility of phenyl alanine in aqueous salt solutions at 20° are
given by Wiirgler (1914) and Pfeiffer and Wurgler (1916).
PHENYLENE DIAMINES o, m, and p. C6H4(NH2)2.
SOLUBILITY IN WATER AT 20°. (Vaubel, 1895.)
100 cc. sat. solution contain 23.8 gms. w'CeH^NI^, d20 of sat. sol. = 1.0317.
loo cc. sat. solution contain 3.7 gms. p C6H4(NH2)2, d20 of sat. sol. = 1.0038.
RATIO OF DISTRIBUTION BETWEEN WATER AND BENZENE AT 25°.
(Farmer and Warth, 1904.)
(Holleman and Rinkes, 1911.)
(Kiister and Wiirfel, 1904-05.)
(Boeseken, 1912.)
(Bramley, 1916.)
(Boeseken, 1912.)
(Crompton and Whitely, 1895.)
(Pawlewski, 1893; Philip, 1903.)
(Jaeger, 1908.)
(Kendall, i<ji4a.)
(Kremann and Rodenis, 1906.)
(Kendall and Carpenter, 1914.)
(Kremann and Rodenis, 1906.)
(Kendall, iyi4a.)
Results for o Phenylene Diamine.
conc. C8Hg
conc. H2O
Results for m Phenylene Diamine.
Gms. o
> Ratio
Gms. m C6H4(NH!1)2 per:
Ratio
conc. C«H«
50 cc. C«H«. 1000 cc. H2O. 50 cc. C6H«. 1000 cc. H2O.
0.0273 0.9818 0.556 0.0828 9.088
0.2040 7-5470 0.541 0.0463 5.260
PHENYL HYDRAZINE C6H6NH.NH2.
RECIPROCAL SOLUBILITY OF PHENYLHYDRAZINE AND WATER, DETERMINED
BY THE FREEZING-POINT METHOD. (Bianksma, 1910.)
Gms.
to C,H6NH.NH2 Soli, p,e
per 100 Gms.
* -
Sat. Sol.
O O Ice
19.8
0.3 2.2 "
20.4
0.6 3.9 "
21.8
0.7 4.6 " +C«H6NH.NH2.JH2O
23
I 4.7 C,HsNH.NH2.iH20
24.2
7 6
26.1
ii. 6 7
26.2
15 8
25-7
16.8 9.6
23-2
19.6 10.9 "
i7
16.6
Gms.
QH6NH.NH2
per loo Gms.
Sat. Sol.
60
Solid Phase.
64
75
79
83
1 C,H6NH.NH,.iH,O
2 "
2 "
7 "
92-3
93-7
97-2
98.8
99
+C6H8NH.NH,
C6H6NH.NH2
19.6 m. pt. ioo . .
Between the concentrations 10.9 and 60. i, two liquid layers are formed. See
p. 487.
487 PHENYL HYDRAZINE
RECIPROCAL SOLUBILITY OF PHENYL HYDRAZINE AND WATER. (Con.)
The temperatures of separation into two liquid layers of mixtures containing
from 10.9 to 60 per cent C6H6NH.NH2, are:
toof Cms. C6H5NH.NH2 t«, Of Gms^C.HjNH.NH, t, Qj Cms. C6H5NH.NH2
19.8 ii. 6 54.6 29.7 50.6 48.9
34 I3-8 55-1 31-4 50 5!-2
45 l6-5 55-a.cnt.-t 33-6 46 53-5
49-4 18.7 55.2 36.9 44.2 54.7
52.4 21.9 55 39-3 39-6 56.7
54 25.2 54 41-7 24 59.5
54.4 28.3 52.6 46 19.8 60. i
Additional data for concentrations of CeHsNH.NH-j above 60 per cent, are given
by Oddo (1913)-
Benzoyl PHENYL HYDRAZINE C6H6NH.NHC7H5O.
SOLUBILITY IN AQUEOUS ALCOHOL AT 25°.
(Holleman and Ajitusch, 1894.)
Cms. Hydrazine cn p- Vnl % Cms. Hydrazin*
ico 2.39 0.793 8o J-59 0.859
95 2.43 0.814 70 i. 08 0.884
93 3 °-822 55 0.51 0.917
90 2.26 0.831 40 0.16 0.946
The above results give an irregular curve. See remarks under a acetnaph-
thalide, p. 13.
XCOV H
Phthalyl PHENYL HYDRAZIDE C6H4< >N.N<
CO CeHfi.
CO^ CH3
Phthalyl PHENYL Methyl HYDRAZIDE C6H4< > N.N (
^CO' ^ C6H5.
Very careful determinations of the solubilities of the enantrotropic forms of
these two compounds in alcohol, chloroform, ethyl acetate, acetone, benzene and
in methyl alcohol are given by Chattaway and Lambert (1915). See also p. 312.
Acetone PHENYL HYDRAZONE (CH3)2C.N2HC6H5.
DATA FOR THE SYSTEM ACETONE PHENYL HYDRAZONE -f- WATER ARE GIVEN
BY BLANKSMA (1912).
The following results were obtained for the solubility of (CHs^C.
in water.
t°.
Cms. (CH3)2C.N2.HC,HS
pet loo cc. Solution.
Solid Phase.
0
0.090
(CHa)2C.N2 HCeHB.HjO
15
0.187
«
32.8
0.412 x
"
DibromoPHENYL SELENIDE and TELLURIDE (Ce
Data for the solubility of mixtures of dibromophenyl selenide and dibromo-
phenyl telluride in benzene at 21° are given by Pellini (1906).
PHLOROGLTTCINOL 1.2.3 C6H3(OH)3.2H2O.
ioogms.H2O dissolve i.i3gms.phloroglucinolat2O-25°. (Dehn, '17.)
" pyridine " 296
" aq. 50% pyridine " 134
PHOSPHO MOLYBDIC ACID 488
PHOSPHO MOLYBDIC ACID P2O5.2oMoO3.52H2O.
SOLUBILITY IN ETHER. (Parmentier, 1887.)
t°. o°. 8.1°. 19.3°.
Cms. Acid per 100 gms. Ether 80 . 6 84 . 7 96 . 7
PHOSPHORUS P. (yellow)
SOLUBILITY IN BENZENE.
(Christomanos — Z. anorg. Ch. 45, 136, ^55.)
«.o Gms. P per Sp. Gr. of
* 100 Gms. C6He. Solution.
AO Gms. P per Sp. Gr. of
' jooGms.CeHe. Solution.
0
1-5*3
. . .
23
3-399
0.8875
5
1.99
. . .
25
3-7o
0.8861
8
2.31
0.8990
30
4.60
10
2.4
0.8985
35
5-17
15
2.7
0.894
40
5-75
18
3-i
0.892
45
6. ii
20
3-2
0.890
27-4-
103.9
32.9°.
107.9
Gmi. P
100 Gms.
50
55
60
65
70
75
81
6.80
7.32
7.90
8-40
8.90
9.40
10.03
SOLUBILITY OF PHOSPHORUS IN ETHER.
10
(Christomanos.)
Gms. P per
100 Gms.
(C2H6)20.
Sp. Gr. of
Solutions.
Gms. P per c f t
f. -a-.; <&$£
Gms. P per
t °. zoo Gms.
(C2H6)20.
0-434
15
0.90
0.723
28
i .60
O.62
. . .
18
I -OI
0.719
30
i .75
0.79
0.732
20
1.04
0.718
33
i. 80
0.85
0.729
23
1. 12
0.722
35
2.00
25
i-39
0.728
SOLUBILITY OF YELLOW PHOSPHORUS IN SEVERAL SOLVENTS AT 15°.
(Stich, 1903.)
Gms. P per
Solut
Solvent.
er 100 Gms.
lution.
Almond Oil 1.25
Oleic Acid i . 06
Paraffin 1.45
Water o . 0003
Acetic Acid (96%) o . 105
SOLUBILITY OF PHOSPHORUS IN CARBON DISULFIDE.
(Cohn and Inouye, 1910.)
— IO
-7-5
-5
Gms. P
per 100 Gms.
Sat. Sol.
31.40
35.85
41-95
-3-5
-3.2
-2-5
Gms. P
per 100 Gms.
Sat. Sol.
66.14
71.72
75
o
+5
IO
Gms. P
per TOO Gms.
Sat. Sol.
8l.27
86.3
89.8
The above determinations were made with very great care. The authors show
that the previous determinations of Giran (1903) are inaccurate.
loogms. alcohol (d = 0.799) dissolve 0.312 gm. P, cold, and 0.416 gm., hot. (Buchner )
100 gms. glycerol (d^ = 1.256) dissolve 0.25 gms. Pat 15-16°. (Ossendowski, 1907.)
Red phosphorus is completely insoluble in turpentine even up to 270° provided
the determination is made without access of air (sealed tube). If air is not ex-
cluded a portion of the red phosphorus may be converted to yellow phosphorus
which would dissolve. (Colson, 1907.)
489
PHOSPHORUS
RECIPROCAL SOLUBILITY OF PHOSPHORUS AND SULFUR, DETERMINED BY
THE SYNTHETIC (Sealed Tube) METHOD.
(Giran, 1906.)
(Mixtures of P and S were sealed in small tubes and first heated to about 200°
to cause combination. They were then cooled to the solidification point and
gradually heated to the temperature at which the last crystal disappeared. The
following results, which were read from the diagram, show the eutectics and
maxima of the curves.)
Eutectics.
t°.
Mols. % S in
Mixture.
Selid Phase.
-40
33-5
P4S3+P2
+46
50
P4S3+P2S3
230
67-5
P2S3+P2S6
243
75
P2S6+PS6
Maxima of Curves.
«•• MMixt?reSiQ Solid Phase.
+ 167 43.6
296
60.8
272
314
72.1
86.1
P2S3
P2S5
PS,
Additional data for this system are given by Boulouch (1902 and 1906) and by
Helff, 1893.
PHOSPHORUS SULFIDES P4S3, P4S7, P4Si0.
SOLUBILITY IN CARBON DISULFIDE, BENZENE, AND IN TOLUENE.
(Stock, 1910.)
Cms. P4S3 per 100 Cms.:
ll .
€82.
CeHs.
C6H6Cn3.
— 20
II .1
0
+17
80
27
100
2-5
II. I
3-125
no
15-4
Cms. P4S7_per 100 Cms. PjS10 per
Gms. €82.
Cms. CSj.
0.005
0.0286
0.083
0.182
0.223
PHOSPHORIC ACID (ortho) H3PO4.
SOLUBILITY IN WATER.
(The sat. solutions were analyzed by titration.
stirred for at least two hours.)
(Smith and Menzies, 1909.)
The mixtures were constantly
Gms. H3PO4
t°. per too Gms. Solid Phase.
Sat. Sol.
-81*
62.9
Ice+2HsPO4.H2O
-16.3
76.7
aH«PO4.HjO
+ o-5
78.7
"
14-95.
81.7
"
24.03
85-7
"
27
87.7
"
29-15
9°-5
"
29-35!
91.6
"
28.5
92-S
"
27
93-4
"
25-4
94.1
"
23-5*
. . .
" +ioH3PO4.H2O
24.11
94.78
ioH3PO4.H2O
Gms. H3PO4
t°. per 100 Gms.
Solid Ph
Sat. Sol.
24.38 94.80
ioH8PO4.H2O
24.40 94.84
"
24.81 -94-95
a
25.41 95.26
«
25-85 95.54
"
26.2*
«
26 . 23 95 . 90
H.PC
27.02 95.98
K
29.42 96.15
M
29.77 96.11
"
37.65 97.80
"
39.35 98.48
«
42.30! 100
«
+H3P04
* Eutec. t M. pt.
NOTE. — The results of Giran (1908), determined by the freezing-point method,
are shown to be erroneous, due to supercooling which would result from failure to
induce crystallization by inoculation.
F.-pt. data for mixtures of phosphoric and phosphorus acids are given by Rosen-
hejm, Stadler and Jakobsohn (1906).
ns. H4PA per ico
Gms. Sat. Sol.
Solid Phase.
59
86.8
Ice +H4PA.i^H20
88.8
+H4PA
100
IL.PA
PHOSPHORIC ACID 490
PyroPHOSPHORIC ACID H4P2O7.
SOLUBILITY IN WATER. (Giran, 1908; see note on preceding page.)
t°.
-75
+26 m. pt.
23
61 m. pt.
HypoPHOSPHORIC ACID H2PO3.H2O.
100 gms. sat. solution in water contain 81.8 gms. H2PO3 at the m. pt., 62°, of
the hydrated compound, t^POa.HgO. (Rosenheim and Pritze, 1908.)
PHTHALIC ACIDS C6H4(COOH)2, o, m and p.
SOLUBILITY OF EACH IN WATER. (Vaubel, 1895, 1899.)
Acid. t°. Gms. per 100 Gms. Solution.
o Phthalic Acid 14 o . 54
m = Isophthalic Acid 25 0.013
p = Terephthalic Acid . . . almost insoluble
MELTING TEMPERATURES OF MIXTURES OF o PHTHALIC ACID AND WATER.
(Flaschner and Rankin, 1910.)
(The determinations were made by the sealed tube method of Alexejew.)
Wt. %Acid 14.4 28.2 39.6 49.3 75 100
Saturation Temp. 97° 111.5° 121.2° 130° 162° 231°
Unstable boundary ... ... ... 27° 84°
SOLUBILITY OF o PHTHALIC ACID IN ALCOHOL AND IN ETHER AT 15°.
(Bourgoin, 1878.)
Gms. C6H4(COOH)2 o per 100 Gms.
Solution.
Solvent.
Absolute Alcohol
9.156
II .70
90 per cent Alcohol
10.478
IO.O8
Ether
0.679
0.684
SOLUBILITY OF o PHTHALIC ACID
IN ALCOHOLS. (Timofeiew, 1894.)
Gms. o
Gms. o
Alcohol t° CeH4(COOH)j
Alcohol.
to C6H4(COOH)2
per 100 Gms.
per 100 Gms.
Sat. Sol.
Sat. Sol.
Methyl Alcohol —2 15.1
Ethyl Alcohol
21.4 11.65
+ 19 19.5
Propyl Alcohol
- 3 3-42
+ 21.4 20.4
« «
+ 19 5.27
Ethyl Alcohol -2 8.2
(( ((
22 5-54
+ 19 ii
(i a
23 5-70
DISTRIBUTION OF o PHTHALIC ACID AND OF m PHTHALIC ACID (ISOPHTHALIC)
BETWEEN WATER AND ETHER AT 25°. (Chandler, 1908.)
Results for o Phthalic Acid. Results for m Phthalic Acid.
Mols. o C,H4(COOH)2 Ratio for Mols. m C6H4(COOH)2 Ratio for
I** Liter: ?- U°n- Per L*er: U'
Ratio- £°n- Per ao-
HtO Layer, a. Ether Layer, 6. Acid. H2O Layer, a. Ether LayerA Acid.
0.0261 0.0322 0.809 0.637 0.000398 0.0485 0.0821 0.0359
0.0131 0.0150 0.873 0.645 0.000272 0.0288 0.0943 0.0352
0.0085 0.0091 0.932 0.667 0.000263 0.0279 0.0944 0.0350
0.0056 0.0056 I. 006 0.635 0.000252 0.0266 0.0949 0.0341
Ratio of solubilities of Phthalic acids in olive oil and water at 25°.
(Boeseken and Waterman, 1911, 1912.)
o Phthalic acid, solubility in oil -s- solubility in H2O = o.oi.
p Phthalic acid (Terephthalic), solubility in oil 4- solubility in H2O = 9.52.
loo gms. 95% formic acid dissolve 0.55 gm. p phthalic acid (Terephthalic) at
20.2°. CAschan, 1913.)
491 PHTHALIC ACIDS
NitroPHTHALIC ACIDS o and m (Iso) C6H3(NO2)(COOH)2.
SOLUBILITY OF THE SEVERAL NITRO PHTHALIC ACIDS itf WATER AT 25°.
(Holleman and Huisinga, 1908.)
Gms. Acid
Acid. M. pt. per 100 Gms.
Sat. Solution.
a. Nitro Ortho Phthalic Acid 220 2 .048
8 " 164-166 very soluble
Symmetrical Nitro Iso Phthalic Acid (anhy.) 255-256 0.220
" (hydrated) 255-256 0.157
Asymmetrical " " " 245 0.967
Vicinal 300 0.216
The authors also give several tables showing the solubility of one of the above
compounds in aqueous solutions of another. These data are .made the basis of
an ingenious solubility method for determining the composition of unknown
mixtures of these compounds.
PHTHALIC ANHYDRIDE C6H4<£g>O.
SOLUBILITY IN WATER.
(van der Stadt, 1902.)
All determinations, except first three, made by the Synthetic Method. See
p. 16.
Gms. C8H4O3 per 100 Gms.
Mol. per cent to
C8HA. * •
Gms. C8H4O3 per
100 Gms
Mol.
percent
C8H40,.
Water.
Solution.
Water.
Solution.
0
O
.00295
O.OO295
o
.00036
189
•5
1076
91
.66
56.73
25
0
.6194
0.6150
0
•P754
188
.8
1265
92
.68
60.63
50
I
.630
1.604
o
.198
187
.1
1474
93
-65
64.22
135-9
94
-3
48.54
10
•30
181
.8
2332
95
.88
73-95
165.4
210
67.75
20
-36
176
.2
3334
97
.07
80.23
179.4
319
•3
76.13
27
.98
169
-4
5745
98
.28
87.49
186.2
449
.6
81.81
35-37
130
•9
37570
99
.72
97.89
189.6
546
.1
84.50
39
•93
83010
99
.86
99.02
191
821
•5
89.19
5o
131
.2
00
100
IOO
190.4
863
•4
89.62
51
.24
SOLUBILITY OF PHTHALIC ANHYDRIDE IN CARBON BISULFIDE.
(Arctowski, 1895; Etard, 1894.)
Gms.
t°. per loo Gms.
Solution.
70 2.3
90 3-7
loo 5
120 8
140 13-3
160 20.7
180 30.2
100 gms. 95% formic acid dissolve 4.67 gms. phthalic anhydride at 19.8°.
(Aschan, 1913.)
loo gms. pyridine dissolve 83.5 gms. phthalic anhydride at 20-25°. (Dehn, 1917.)
r.
Gms. C8H4O3
per loo Gms.
Solution.
f.
per 100 Gms.
Solution.
-112.5
0.013
+ 10
0.3
-93
-77-5
0.013
0.016
20
30
0.7
0.8
-40
— 20
— 10
0.03
0.06
O.IO
40
50
60
1.2
0
0.20
PHTHALIMIDE 492
PHTHALIMIDE o C6H4 < (CO)2 > NH.
100 gms. H2O dissolve 0.06 gm. phthalimide at 20-25°. (Dehn, 1917.)
" pyridine " 14.15 gms. "
" aq. 50% pyridine 7-74
PHTHALONIC ACID COOH.C6H4.CO.COOH.2H2O.
100 gms. sat. solution in water contain'64.4 gms. anhydrous acid at 15°, Sp. Gr.
of sat. solution = 1.243. (Tcherniac, 1916.)
Amide of PHTHALIDECARBOXYLIC ACID C6H4<SS(CONH2) >O (m. pt.
185.5°).
100 gms. H2O dissolve 0.132 gm. of the acid at 16.2° and 5.7 gms. at b. pt.
(Tcherniac, 1916.)
PHYSOSTIGMINE (Eserine) Ci5H21N3O2.
Water dissolves only traces of physostigmine. ipo gms. of a solvent composed
of 3 gms. H3BO3 per 100 cc. of aq. 50% glycerol dissolve 2.5 gms. Ci5H2iN3O2 at
room temp. (Baroni and Borlinetto, 1911.)
PHYSOSTIGMINE SALICYLATE C6H4(OH)COOH.Ci6H21N3O2 and Physo-
stigmine Sulfate H2SO4(Ci5H2iN3O2)2.
SOLUBILITY OF EACH IN WATER, ALCOHOL, ETC.
(U. S. P. VIII.)
Salicylate.
Sulfate.
Water
25 I-38
very soluble
Water
80 6.66
u
Alcohol
25 7-87
((
Alcohol
60 25
{(
Chloroform
25 ii. 6
((
Ether
25 0.57
0.083
Methylphenyl PICRAMIDES.
SOLUBILITY
IN ETHYL ALCOHOL
AT 18°.
(Hantzsch, 1911.)
100 cc. C2H6OH dissolve 0.32 gm. of the isomer melting at 108°.
100 cc. C2H6OH dissolve 0.42 gm. of the isomer melting at 128°.
PICRIC ACID C6H2.OH.(NO2)3 1.2.4.6.
SOLUBILITY IN WATER.
(Dolinski — Ber. 38, 1836, '05; Findlay — J. Ch. Soc. 81, 1219, 'oa.)
Gms. CeHsNsO? per 100 Grams Gms. CeHsNaO? per 100 Grams
Solution.
Water.
Solution.
Water.
0
0.67 (D.) 0
.68 (D.) I
.05 (F.)
60
2
• 77 (D.) 2.8l(D.
) 3-i7(F.)
10
.80
o
.81
I
.10
70
3
•35
3
•47
3-89
20
1. 10
I
.11
I
.22
80
4
.22
4
.41
4.66
30
1.38
I
• 40
I
•55
90
5
•44
5
.72
5-49
40
I
.78
I
.98
IOO
6
•75
7
.24
6-33
50
2.15
2
.19
2
•53
. Dolinski does not refer to the previous determinations of Findlay.
loo gms. H2O dissolve 1.525 gms. C6H2.OH.(NO2)3 at 30° and 1.868 gms. at 40°.
(Karplus, 1907.)
loo gms. H2O dissolve 1.45 gms. C6H2.OH.(NO2)3 at 20°. (Sisley, 1902.)
loo gms H2O containing 5 gms. H2SO4 per liter, dissolve 0.61 gm. C6H2OH(NO2)3
at 20°. (Sisley, 1902.)
loo gms. ethyl alcohol dissolve 8.37 gms. C6H2OH(NO2)3 at 22°. (Timofeiew, 1894-)
loo gms. methyl alcohol dissolve 22.5 gms. C6H2OH(NO2)3 at 22°.
loo gms. propyl alcohol dissolve 3.81 gms. C6H2OH(NO2)3 at 22°.
loo gms. 95% formic acid dissolve io.83gms. C6H2OH(NO2)3at 19.8°. (Aschan, 1913.)
493
PICRIC ACID
SOLUBILITY OF PICRIC ACID IN WATER AND IN AQUEOUS SALT
SOLUTIONS AT 25°.
(Levin — Z. physik. Ch. 55, 520, '06.)
One liter of aqueous solution contains 0.05328 gram mols. = 12.20
grams C6H2.OH(NO2)3 at 25°.
Gm Mols Salt Gram Mols. Picric Acid per Liter in Aq. Solutions of:
per
Liter.
'NaCl.
NaNO3.
Na2SO4.
LiCl.
Li2S04.
NIL^Cl.
0
.01
0
•05524
0.05529
0-05604
0.05480
O
.05661
0.05487
O
• O2
o
•05559
0-05872
0.05872
0-05558
0
.06053
0.05540
0
•05
o
.05729
0.06632
0.06632
0.05703
0
.06691
0.05771
0
.07
0
.05862
6.07093
0.07093
0.05878
o
.07013
0.05865
O
.10
0
.05902
0.07670
0-07670
0.06132
o
•07437
O
•50
o
.0790
0
.123
I
.00
o
.Il8o
...
0
.149
Gm.
, Mols.
Grams Picric Acid per
Liter in Aq. Solutions of:
Salt per Liter.
NaCl.
NaNO3.
Na2S04.
; uci.
Li2S04.
NH«C1.
O
.01
12.66
12.67
12.83
12 .55
12-97
12-57
O
• O2
12.74
13-45
13-45
12-74
I3-87
12.69
0
•05
13.12
13.06
15-33
13.22
O
.07
13-43
16.25
16.25
13-47
16.06
13-44
O
.10
13-52
17-57
17-57
14.05
17.04
0
•50
18.09
28.18
I
.00
26.98
•
34-14
Solubility in Aq. Cane Sugar.
Solubility in Aq. Grape Sugar.
Gm. Mols.
Sugar
per Liter.
Picric Ac. per Liter Solution.
Sp. Gr.
Solution.
Gm. Mols.
Grape Sugar
per Liter.
Picric Acid
£er Liter Sol.
Gm. Mols.
Cms.
G. Mols.
Gms.
O-IO
0.05202
II .92
I .OI22
O.IO
0.0530
12.14
0.25
0.04978
11.40
I.03I9
0.25
0.0521
"•93
0.50
0.0482
II .04
I .0654
0.50
0-0509
11.66
1. 00
0.0443
IO.I5
I.I294
I .OO
0-0474
10.86
SOLUBILITY OF PICRIC ACID IN ABSOLUTE ALCOHOL.
(Behrend — Z. physik: Ch. 10, 265, '92.)
TOO gms. sat. solution contain 5.53 grams CeHgNgOj at 12.3°, and
5.92 grams at 14.8°. Sp. Gr. of the latter solution = 0.8255.
SOLUBILITY OF PICRIC ACID IN BENZENE.
(Findky.)
Gms.
Mols.
t*.
C6H3N307
C6H3N3O
per 100
Gms.C6H6.
per 100
Mols.CsE
5
3-70
1.26
10
5-37
I .83
'5
7-29
2.48
20
9.56
3-25
25
12.66
4-30
26.5
13 -51
4.60
35
21.38
7.26
Gms.
Mols.
per 100 per 100
Gms.CeHe. Mols. ~ "
38.4
26.15
8.88
45
33-57
ii .40
55
50-65
17.21
58.7
58-42
19.83
65
71 .31
24.20
75
96.77
32.92
PICRIC ACID 494
SOLUBILITY OF PICRIC ACID IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID AT 25°.
(Stepanow, 1910.)
(The solutions were saturated by constant agitation at constant temperature.
The picric acid in the saturated solutions was determined by evaporation and
weighing. The solubility passes through a minimum.)
Mols. HC1
C6H2.OH.(]
\Oz)s per Liter.
Mols. HC1
C6H2.OH.(N02)3
per Liter.
per Liter.
Mols.
Cms.
per Liter.
Mols.
Cms.
0.25
0.0116
2.66
3^7
0.0068
i-SS
0.50
0.0079
i. 80
4.40
0.0082
1.87
o-7S
0.0062
1.42
5-H
o . 0098
2.26
i
0.0054
1.24
5-51
O.OIO5
2.41
1.47
0.0050
1.14
5-87
O.OII5
2.65
2.20
0.0051
i-i5
6.24
0.0123
2.82
2.94
0.0057
i-3i
6.61
O.OI25
2.86
SOLUBILITY OF PICRIC ACID IN ETHER.
(Bougault, 1903.)
Solvent. t°. Cms. CeHjNsOr per Liter'
Ether of Sp. Gr. 0.721 13 10.8 (B.)
Ether of Sp. Gr. 0.725 (0.8 pt.H2O per 100) 13 36 .8
Ether of Sp. Gr. 0.726 (i pt. H2O per 100) 13 40
Ether saturated with H2O 15 51 .2
H2O saturated with Ether 15 13.8
100 parts of ether dissolve about 2.27 gms. picric acid at 15°. (S. 1905.)
chloroform 2
" petroleum ether 0.04 '
loo gms. sat. solution in pure ether contain 5 gms. picric acid at 20°. (Sisley, 1902.)
100 cc. sat. solution in pure ether contain 3.7 gms. picric acid at 20°.
100 gms. sat. solution in pure toluene contain 12 gms. picric acid at 20°.
100 cc. sat. solution in pure toluene contain 10.28 gms. picric acid at 20°. "
100 cc. sat. solution in pure amy 1 alcohol contain i .755 gms. picric acid at 20°. "
DISTRIBUTION OF PICRIC ACID AT 25° BETWEEN:
Water and Amyl Alcohol. Water and. Toluene,
(Herz and Fischer — Ber. 37, 4747. '04.) (H. and F. — Ber. 38, 1142, '05.)
Millimols CeHjjNsOr
per 10 cc.
Gms. CeHaNgOy
per 100 cc.
Millimols CeHgNaOy
per 10 cc.
Gms. QHgNaOr
per 100 cc.
Aq.
Alcohol "
Aq.
Alcohol
* Aq.
Toluene
Aq.
Toluene
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
0-0553
0.0930
0.127
0.213
0.075
0.126
0.172
0-289
0.0920
0.1850
O.2II
0.424
O.IO9
0.230
0.250
0.527
O.l6l3
0.4127
0.369
0.946
0.163
0.482
o-374
I .IO4
0.1869
0.5182
0-428
I.I88
0.244
I .026
o-559
2-351
0.3l6l
1.079
0.724
2-473
0.389
2-347
0.891
5-38o
0.4471
1.638
I .024
3-753
0.496
3-747
i-i37
8.586
0.5624
2.189
1.288
5-oi7
0.583
5-135
I-336
11.770
0.6423
2-549
1.472
5-839
Additional data for the distribution of picric acid between water and amyl
alcohol and water and toluene at 20° are given by Sisley (1902). Very irregular
results were obtained. The fact that the colors of the two layers are different,
was taken to indicate that the picric acid dissolves in a different molecular form
in the two layers.
495 PICRIC ACID
DISTRIBUTION OF PICRIC ACID AT 25° BETWEEN:
Water and Bromoform. Water and Chloroform.
(Herz and Lewy — Z. Electrochem, n, 820, '05.) (H. and L.)
MiUimols CeHsNaOr Cms. CeHsNaOr Mfflimols QjHsNaOr Cms. QHaNsOr
per 10 cc. per 100 cc. per 10 cc. per 100 cc.
Aq. Bromoform Aq. Bromoform Aq. Chloroform
Layer. Layer. Layer. Layer. Layer. Layer.
0.321 0.365 0.736 0.836 0.207 0.254
0-401 0.515 0.919 I.lSo 0.329 0-547
0-475 °-655 i. 088 1.501 0.488 1.09
o-575 0.871 1.317 1.995 0.561 1.41
0.674 1.14 1.545 2.612 0.588 1.53
DISTRIBUTION OF PICRIC ACID BETWEEN:
Water and Benzene. (Kuriloff, 1898.) Water and Ether at 20°.
Mols. Picric Acid per Liter: Cms. Picric Acid per Liter:
Aq. Chloroform
Layer. Layer.
0.474 0.582
o-754 1-253
1.118 2.498
1-285 3-230
1-348 3-505
(Sisley, 1902.)
Dist. Coef.
2.63
i-79
i-34
0.13
O.OI
Aq. Layer. C6H6Xayer.
0.026l 0.0940
O.O2O8 0.0779
0.0188 0.0618
0.0132 0.0359
0.0097 0.0198 1 L
Aq. Layer. Ether Layer.
6.78 17.85
3.74 6.70
2.85 3.72
0.85 o.n
O.IO O.OOI
Data for the distribution of picric acid between water and mixtures of chloro-
form and toluene at 25°, are given by Herz and Kurzer (1910).
FREEZING-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR
THE FOLLOWING MIXTURES:
Picric Acid + Dirnethylpyrone. (Kendall, 1914.)
-j- Resorcinol. (Philip and Smith, 1905.)
-J- Thymol. (Kendall, 1916.)
+ a Trinitrotoluene. (Giua, 1916.)
MethylPICRIC ACID C6H(CH3)(OH)(NO2)3, 1.3.2.4.6.
SOLUBILITY IN AQUEOUS SOLUTIONS AT 25°. (Kendall, 1911.)
Normality of Normality of
A c i Dissolved A c i «• Dissolved
Aq. Solvent. Methyl pkric Aq. Solvent. Methyl picric
Acid. Acid.
Water o.oioo 0.01975 n o Nitrobenzoic Acid 0.0080
" -f-Ligroin 0.01019 0.00981 n Salicylic Acid 0.01063
" -(-Toluene 0.01059 0.01393 n " 0.01072 .
0.00895 n HC1 0.00641 H2O+Excess of Salicylic Acid 0.02613*
0.01593 n HC1 0.00487
0.01013 n Picric Acid 0.00702
* = normality of salicylic acid + inethylpicric acid.
PICROTOXIN C3oH34013.
loogms. H2O dissolve o.4i+gm. picrotoxin at 20-25°. (Dehn, 1917.)
pyridine dissolve 102 gms. "
aq-50%pyridine 81
PIMELIC ACID (CH2)5(COOH)2.
DISTRIBUTION BETWEEN WATER AND ETHER AT 25°. (Chandler, 1908.)
Mols. (CH2)5(COOH)j per Liter.
Dist. Coef. ?
1
0.7095
0.7170
0.7195
o . 7480
0.7075
Dist. Coef.
Corrected
for lonization.
0.670
0.670
0.663
0.663
0-653
Aq. Layer, a.
o . 00998
0.00702
0.00480
O.OO284
O.OOI79
Ether Layer, b,
O.OI4O7
0.00979
0.00667
0.00380
0.00253
PILOCARPINE 496
PILOCARPINE CUH16N202.
100 cc. oil of sesame dissolve 0.3142 gm. CnHi6N2O2 at 20°. (Zalai, 1910.)
PILOCARPINE HYDROCHLORIDE CUH16N2O2.HC1, Pilocarpine Nitrate
CiiHi6N2O2.HNO3, and Piperine Ci7H19NO3 in Several Solvents.
(U. S. P., VIII.)
Gms. per 100 Gms. Solvent.
Solvent. t°. , » x
CUH16N202.HC1. CUH16N202.HN03. ,C17H19NO,.
Water 25 333 25 insoluble
Alcohol 25 4-35 1-66 6.66
Alcohol 60 9.09 6.2 22.7
Chloroform 25 0.18 ... 58.8
Ether 25 ... ... 2.8
PINACOLIN CH3.CO.C(CH3)3.
SOLUBILITY IN WATER AND IN AQ. ACETONE AT 15°. (Deiange, 1908.)
Per cent Acetone cc. Pinacolin Dissolved
in Solvent. per 100 cc. Solvent.
o (= pure H2O) 2 .44
20 3.47
33 6.06
50 9.09
60 14-27
PINENE HYDROCHLORIDE C10H16.HC1.
IOO gms. 95% formic acid dissolve i.2gms. CioHie.HCl at 16.8°. (Aschan, 1913.)
PIPECOLINE C5H9(CH3)NH d and /.
F.-pt. data for mixtures of d and I pipecoline are given by Ladenburg and
Sobecki (1910).
PIPERIDINE CH2<(CH2.CH2)2>NH.
DISTRIBUTION BETWEEN WATER AND BENZENE AT ORD. TEMP. (Georgievks, 1915.)
Gms. Piperidine per: Gms. Piperidine per:
25 cc. H2O Layer. 75 cc. C6H6 Layer. 25 cc. H2O Layer. 75 cc. CeH6 Layer.
0.1573 0.4127 0.891 2.339
0.256 0.674 1.299 3-589
0.409 I. 088 I.7I2 4-789
0.674 1-746
PIPERIDINE HYDROCHLORIDE CH2<(CH2.CH2)2>NH.HC1.
SOLUBILITY IN SEVERAL SOLVENTS. (Freundiich and Richards, 1912.)
c,o,ro, *o Mols. Piperidine
Solvent. * • HC1 per Liter.
Water o 4.87
25 S-iQ
Tetrachlor Ethane (sat. with H20) o 0.13
25 0.29
Nitrobenzene 25 0.00543
Benzene 25 0.00102
MethylPIPERIDINES 2-, 3-, 4-, n Methyl, etc.
Data for the reciprocal solubility of 2-methylpiperidine and water, 3-methyl-
piperidine and water, 4-methylpiperidine and water, nitrosopiperidine and water
and for w-methylpiperidine and water, determined by the synthetic (sealed tube)
method of Alexejeff, are given by Flaschner and MacEwan (1908) and by Flasch-
ner (1909) and (1908). Similar data for «-ethylpiperidine and water and for n-
propylpiperidine and water are given by Flaschner (1908).
497 PIPERIDINES
act' Diphenyl PIPERIDINES Ci7Hi9N.
SOLUBILITIES OF THE ACID SALTS OF ace' DIPHENYL PIPERIDINE AND OF I so act'
DIPHENYL PIPERIDINE IN WATER AT 25°.
(Scholtz, 1901.)
Cms. per 100 Cms. Sat. Solution:
Piperidine Base. f - • — • - * - \
HClSalt. HBrSalt. HI Salt. H2SO4 Salt.
a, a' Diphenyl Piperidine, m. pt. 7 1° o . 85 o . 90 0.12 6.31
Iso a, a' Diphenyl Piperidine, liquid 3.02 i 0.72 easily soluble
PIPERINE Ci7Hi9N03. (See also under Pilocarpine, preceding page.)
SOLUBILITY IN SEVERAL SOLVENTS.
! Authority.
Water 20-25 0.01 (Dehn, 1917.)
Ethyl Alcohol 9.5 2.9 (Timofeiew, 1894.)
Methyl " 9.5 4.4
Propyl " 9.5 2.94
Trichlor Ethylene 15 9 . 83 (Wester and Bruins, 1914-)
Pyridine 20-25 22.46 (Dehn, 1917.)
Aq. 50% Pyridine 20-25 IJ-39
PLATINUM ALLOYS.
SOLUBILITY OF PLATINUM ALLOYS IN NITRIC ACID.
(Winkler — Z. anal. Ch. 13, 369, '74.)
Appro*. Grams Alloy Dissolved per TOO Grams HNOs Solution of
Pt^in Alloy. ^
i.3o8Sp.Gr.
i.2o8Sp.Gr.
i.iooSp.Gr.
i.2o8Sp.Gr4
IO
57
44
69
37
5
69
57
51
35
2-5
62
61
69
I
75
70
76
10
46
27
II
51
5
36
34
14
4i
2-5
51
40
30
i
52
41
37
. .
10
7
9
8
5
8
9
10
..
2-5
22
17
ii
21
18
23
.-.
10
14
19
4
3
5
21
20
6
18
2-5
25
42
8
I
49
64
10
...-. •
10
10
II
19
5
5
16
12
6
ii
2-5
16
24
19
..
i
20
32
37
Pt and Silver
Pt and Copper
Pt and Lead
n
M
II
Pt and Bismuth
Pt and Zinc
ii
n
ii
PLATINUM BROMIDE PtBr4.
100 grams sat. aqueous solution contain 0.41 gram PtBr4 at 20°.
(Halberstadt — Ber. 17, 2062, '84.)
PLATINIO POTASSIUM BROMIDE K2PtBr6.
100 grams sat. aqueous solution contain 2.02 grams K2PtBr6 at 20°.
(HalberstadU
PLATINUM CHLORIDES
498
PLATINIC DOUBLE CHLORIDES of Ammonium, Caesium, Potassium,
Rubidium and Thallium. (Data for each separately.)
SOLUBILITY IN WATER.
(Crookes — Chem. News 9» 37. 205, '64; Bunsen — Pogg. Ann. 113, 337, *6i.)
Grams per 100 Grams Water.
1".
(NH^tCle.
Cs2PtCl6.
K2PtCl6.
Rb2PtCl6.
Tl2PtCl<j.
0
10
0*666(15°)
O.O24
0.050
o-74
0.90
0.154
0.0064(15°)
20
25
30
40
...
0.079
0.095
O.IIO
0.142
1. 12
1.26
I.4I
I.76
O.I4I
0.143
0.145
0.166
...
£
6o
0.177
0.213
2.17
2 .64
0.203
0-253
. . .
70
0.251
3-19
0-329
80
0.291
3-79
0.417
90
100
1-25
0.332
0-377
4-45
0.521
0-634
0.050
SOLUBILITY OF POTASSIUM CHLOROPLATINATE IN WATER AND IN AQUEOUS
SOLUTIONS OF POTASSIUM CHLORIDE AND OF SODIUM CHLORIDE.
(Archibald, Wilcox and Buckley, 1908.)
Solubility in Water.
Gms. K2PtCl«
t°. per 100 Gms.
H20.
0.4784
0.5992
0.7742
O
IO
20
30
40
60
80
100
355
444
In Aq. KC1 at 20°.
Gm. Mols. Cms. K2PtCl«
5-030
KCl
per zoo Gms.
>er Liter.
Solvent.
O.2C
0.0236
0.25
O.O2O7
0.50
0.0109
I
o . 0046
2
O.OO45
3
O.OO43
4
0.0042
sat.
0.0034
In Aq.
NaCl at 1 6°.
Gm. Mols. Cms. K2PtCU
NaCl
per loo Gms.
per Liter
Solvent.
0
0.672
0.05
0.700
0.10
0.729
0.25
0.758
0.50
0-775
o-7S
0.791
i
0.805
2
0.834
SOLUBILITY OF POTASSIUM CHLOROPLATINATE IN AQUEOUS SOLUTIONS OF
METHYL ALCOHOL AND OF &THYL ALCOHOL AT 20°.
(Archibald, Wilcox and Buckley, 1908.)
Wt. Per cent
Alcohol in
Gms. K2PtCl« per 100 Gms.:
Solvent.
Aq. CHjOH.
Aq. C2H5OH.
0
0.7742
0.7742
5
0-535
0.491
10
0.412
0.372
20
0.264
0.218
30
0.1831
0.134
40
O.II65
0.076
Wt. Per cent
Alcohol in
Solvent.
50
60
70
80
90
100
Gms. K2PtCl8 per 100 Gms.:
Aq. CH3OH.
Aq. C2HSOH.
0.0625
0.0491
0.0325
0.0265
0.0l82
0.0128
0.0124
0.0085
0.0038
0.0025
O.OO27
o . 0009
loo gms. aq. 8.2% isobutyl alcohol dissolve 0.625 Sm- K2PtCl6 at 20°.
loo gms. aq. sat. isobutyl alcohol dissolve 0.318 gm. K2PtCl6 at 20°.
(Archibald, Wilcox and Buckley, 1908.)
One liter of 55% alcohol dissolves 0.150 gm. (NH4)2PtCl6at 15-20°. (Fresenius, 1846.)
76% " " 0.067 "
95% " " 0.0037 "
499 PLATINUM CHLORIDES
DISTRIBUTION OF PLATINUM CHLORIDE BETWEEN WATER AND ETHER AT
ORD. TEMP. (Mylius, 1911.)
When i gm. of platinum as chloride is dissolved in 100 cc. of aq. 10% HC1 and
shaken with 100 cc. of ether, o.oi per cent of the platinum enters the etheral layer.
If water is used instead of 10% HC1, approximately the same per cent of Pt enters
the ether layer.
100 cc. anhydrous hydrazine dissolve I gm. platinic chloride, with formation of
a black precipitate at room temp. (Welsh and Broderson, 1915.)
ChloroPLATINATES of Hydrocarbon Sulfines.
SOLUBILITY OF EACH IN WATER AT 16°. (Stromholm, 1900.)
Chloroplatinate. Cms. Salt per
f • • — •* \ 100 Gms.
Name. Formula. Sat. Solution.
Trimethyl Sulfine Chloroplatinate
Dimethyl Ethyl Sulfine Chloroplatinate
Methyl Diethyl Sulfine Chloroplatinate
Triethyl Sulfine Chloroplatinate
(CH3)3S]2PtCl6 0.47
(CH3)2(C2H5)S]2PtCl6 3-43
CH3(C2H5)2S12PtCl6 2.42
(C2H5)3S]2PtCl6 1.98
Similar results for more complex sulfines are also given.
PLATING AMINES.
SOLUBILITY IN WATER. (Cleve, 1866 ?)
Amine. Formula. Gms. per 100 Gms. H2O.
Platino Semi Diamine Chloride pt< (NH.),.C1 0. 26 at 0°, 3 . 4 at 100°
Chloro Platino Amine Chloride OPt < *gjg o. 14 at o°, 3 at 100°
Chloro Platino Semi Diamine Chloride Cl3Pt(NH3)2Cl o . 33 at o°, i . 54 at 100°
PLATINOUS NITRITE AMMONIUM COMPOUNDS.
SOLUBILITY IN WATER. (Tschugaev and Kiltinovie, 1916.)
When ammonia is added to a cold solution of potassium platinonitrite a copious
precipitate of the composition Pt2NH3(NO2)2, is obtained. By comparison of
the solubility of this precipitate with that of each of three hitherto described
ammonioplatinum compounds, it 'was found that the precipitate obtained as de-
NH3. .N02
scribed, corresponds to the cis form of dinitro diammonio platinum, / Pt (
NH3 NO2
The results for the solubility of cis and trans dinitro diammonio platinum and of
tetra ammonia platinous platinonitrite in water, are as follows :
Gms. Each Compound per 100 Gms. H2O.
trans Pt2NH3(NO.,)2. [Pt4NH3] [Pt(NOk)4l-
25 0.083 0.063 o.on
63 o . 66 o . 49 ...
74.4 ... 0.81
95 2.32 1.85
Determinations of the solubility of several mixtures of the cis and trans com-
pounds in water are also given.
PONCEAU (Free Acid) Ci0HTN:N.Ci0H4(OH)(SQ,H),.9HiO.
SOLUBILITY IN SEVERAL SOLVENTS AT 23.° (Sisley, 1002.)
Solvent. Gms. Ponceau per Liter.
Water 209 . 6
+5 Gms. H2SO4 per Liter 180
" Sat. with Amyl Alcohol 195
Amyl Alcohol 73 .4
Ether, pure none
Data are also given for the distribution of ponceau between water and amyl
alcohol at 18°.
POTASSIUM
500
POTASSIUM K2.
SOLUBILITY OF POTASSIUM IN LIQUID AMMONIA. (Ruff and Geisei, 1906.)
to Mols. NH3 to Dis-
solve i Gm. Atom K.
— loo 4.82
-So 4-79
o 4.74
SOLUBILITY OF POTASSIUM IN MELTED KOH. (von Hevesy, 1909.)
Difficulty was experienced due to the failure of the excess of K to separate com-
pletely from the saturated solution. Time of heating, 50 hours.
t°. Cms. K per 100 Cms. KOH.
480 7.8-8.9
600 3 -4
650 2 -2.7
700 0.5-1.3
POTASAMMONIUM K?(NH3)2.
100 gms. liquid ammonia dissolve 99.5 gms. K2(NH3)2 at o° and 97 gms. at
+8.44°. (Joannis, 1906.)
POTASSIUM ACETATE CH3COOK.iiH2O.
SOLUBILITY IN WATER. (Abe, 1911.)
• Gms. CHsCOOK
t°. per 100 Gms. Solid Phase.
H20.
2CH3COOK.3H2O
Gms. CH3COOK
per 100 Gms.
H20.
Solid Phase.
O.I 216.7 2CH3COOK.3H2O 41 327-7 2 CH3COOK.3H20
5 223.9 " 4i.3tr.pt. ... " +2CH3cooK.H2o
10 233.9 " 42 329 2CH3COOK.H2O
15 243.1 «« 45 332.2
20 255.6 50 337.3
25 269.4 " 60 350
30 283.8 " 70 364.8
35 30.1-8 " 80 380.1
38 314.2 « 90 396.3
40 323.3 96 406.5
SOLUBILITY OF POTASSIUM ACETATE IN AQ. ALCOHOL SOLUTIONS AT 25°. (Seideii, '10.)
<*25 of Gms. CH3COOK per
Sat. Sol. loo Gms. Solvent.
219.6 70 LI56 Il8.3
219.6 80 1.085 87.6
192.4 90 0.990 52.9
171.8 95 0.922 34.2
147.5 I0° 0.850 16.3
Wt. % QHjOH
in Solvent.
O
20
40
50
60
Sat. Sol.
.417
.363
.302
.260
.210
Gms. CH3COOK per
100 Gms. Solvent.
F.-pt. data for potassium acetate + acetic acid (Vasilev, 1909); potassium
acetate + sodium acetate (Baskov, 1915). (Baskov, 1915.)
POTASSIUM SulfoANTIMONATE
SOLUBILITY IN WATER.
Solid Phase.
Ice
(Donk, 1908.)
' i-3
- 2.6
- 4
- 7.2
— 10.6
-&.$
-28.8
9-5
17.1
24.2
35-4
42.9
48.8
52.6
59-6
t o Gms. K3SbS4 per
loo Gms. Sat. Sol. Solid Phase.
-34
62
Ice+K3SbS4.6H2O
— 10
65.5
K3SbS4.6H20
- 4.5
69.1
"
0
75-4
K3SbS4.sH2O
+ 10
76.2
«
30
75-i
«
50
77-7
K8SbS4.3H20
80
79.2
it
5oi POTASSIUM SulfoANTIMONATE
SOLUBILITY OF POTASSIUM SULFOANTIMONATE IN AQ. SOLUTIONS OF
POTASSIUM HYDROXIDE AT 30° AND VICE VERSA.
(Donk, 1908.)
Gms. per 100 Gms. Sat. Sol.
K3SbS4.
75
68.4
56.8
50-9
37-7
KOH.
O
3-4
ii
16.1
25 5
Solid Phase.
K3SbS4.sH2O
K3SbS4.3H20
K3SbS4
Gms. per 100 Gms. Sat. Sol.
K3SbS4.
19.8
KOH.
40-5
•> OUMU rua,sc.
K3SbS4
"•5
49.9
" +KOH.2H20
9.4
0
49.9
56.3
KOH.2H2O
u
SOLUBILITY OF POTASSIUM SULFOANTIMONATE IN AQ. ETHYL ALCOHOL.
(Donk, 1908.)
Solid Phase.
K3SbS4.sH2O
Results at 10°.
Gms. per roopms. Sat. Sol.
'K3SbS4. QH5OH. '
o 94
o 90.5
Two Liquid Layers Formed Here.
69 . 2 0.8
76.1 o
Composition of the Liquid Layers.
Gms. per 100 Gms.
Results at 30°.
Gms. per 100 Gms. Sat. Sol.
K3SbS4.
O
C2H5OH.
97
Solid Phase.
K3SbS4.3H2O
Two Liquid Layers Formed Here:
Composition of the Liquid Layers.
Gms. per 100 Gms.
Alcoholic Layer.
Aqueous Layer.
K3SbS4.
0
2.2
4.2
27.4
C2H5OH.
85
54-7
46.9
16
"K3SbS4.
67.4
49
45-6
C,HBOH.
I.I
3-4
3-8
Alcoholic Layer.
Aqueous Layer.
K3SbS4.
C2H5OH.
K3SbS4.
QHBOtf.
0
93-i
70.5
±0.5
0
85.6
65.2
I .2
2.2
56.8
47-8
5-7
8.5
41.1
37-i
9-2
12.7 31-1
SOLUBILITY OF POTASSIUM SULFOANTIMONATE IN AQ. METHYL ALCOHOL AT 15°.
(Donk, 1908.)
Composition of the Liquid Layers.
Gms. per 100 Gms.
Gms. per 100 Gms. Sat. Sol. Solid Phase.
K3SbS4. CH3OH.
0.5 99.5 K3SbS4
0-45 99-5
i. 5 93-9
1.8 92
Two Liquid Layers Formed Here.
62.7 7.5 KaSbS^HjO ... ... 31.1 31.3
68.4 3.5 41.1 22.2
75-5 o 47.2 18.2
Two Liquid Layers Formed Here. ... ... 57 -2 II. I
0-5 98.1
POTASSIUM (Dihydrogen) ARSENATE KH2AsO4.
100 gms. sat. aq. solution contain 15.9 gms. KH2AsO4, or 100 gms. H2O dissolve
18.86 gms. at 6°. Sp. Gr. of solution = 1.1134. (Field, 1859.)
100 cc. sat. aq. solution contain 28.24 gms. KH2AsO4 at about 7°.
(Muthmann and Kuntze, 1894.)
loo gms. glycerol (d16 = 1.256) dissolve 50.1 gms. potassium arsenate at 15-16°.
(Ossendowski, 1907.)
Alcoholic Layer.
Aqueous Layer.
'K,SbS4.
5
4-9
13-6
19.1
CH3OH.'
82.5
76.3
66.9
54
45-5
62.5
CH3OH."
8
POTASSIUM BENZOATE 502
POTASSIUM BENZOATE KC7H6O2.3H2O.
SOLUBILITY IN WATER.
(Pajetta, 1906, 1907.)
t°- 17-5° 25° 33-3° 50°
Cms. KC7H602 per ioo Gms. Solution 41.1 42.4 44 46.6
POTASSIUM BORAXES.
SOLUBILITY OF POTASSIUM BORATES IN WATER AT 30°.
(Dukelski — Z. anorg. Chem. 50, 42, '06, complete references given.)
Gms. per ioo Gms. Solution. Gms. per ioo Gms. Residue. Solid
' K20. B203. * K20. B203. ' Phase-
47 . 50 ... ... ... KOH.2H2O
46.36 O.QI 46.13 9-02 K2O.B203.2iH20
40-51 1-25 41.62 9.71
36.82 I. 80 39-90 13 .19.
32-74 3-51 37-22 14.58
29.63 6.98 35.05 17.92
24.84 17-63 30.02 21.70 "
23.30 18.19 26.84 3J-49 K20.2B203.4H20
16.21 13-10 25.12 33 .18
11.78 9.82 20.57 26.43
9.18 8.00 22.38 31-30
6.22 9.13 20-87 31 06
7-73 J3'37 22.21 36.24 K20.2B208.4H20+K20.5B203.8H20
7.81 13.28 17.50 34.18
7.71 13.21 11.49 34 -8l K20.5B203.8H20
7.63 13.28 12.51 4052
3-42 7-59 10.77 37.35
I. 80 4.15 5.88 20-00
0.51 3.19 10.81 40.89
0-33 4-58 7-72 34-21 K20.5B203.8H20+B(OH)a
0.31 4-46 3.91 30-68
3-54
POTASSIUM MetaBORATE KBO2.
Fusion-point data for potassium metaborate + sodium metaborate and for
potassium metaborate + potassium metaphosphate are given by van Klooster
(1910-11).
POTASSIUM PerBORATES, 2KB03.H2O, 2KB03.H2O2.
SOLUBILITY OF EACH IN WATER.
(v. Girsewald and Wolokitin, 1909.)
T>_rat., % Active O in f0 Gms. Salt per ioo
Borate. Gms. Water.
2KBO3.H2O 14.93 ° i-2S
14.93 i5 2.50
2KBO3.H2O2 20.84 15 0.70
POTASSIUM (Fluo) BORIDE KBF4.
ioo gms. H2O dissolve 0.44 gm. KBF4 at 20°, and 6.27 gms. at 100°.
(Stolba, 1889.)
503
POTASSIUM BROMATE
POTASSIUM BROMATE KBrO3.
SOLUBILITY IN WATER.
(Krcmers — Pogg. Ann. 97, 5, '56; Rammelsberg — Ibid. 55, 79, '42; Pohl — Sitzber. Akad. Wiss
Wien. 6, 595, '51-)
Gms. KBrOa per 100 Gms.
f m
' Water.
Solutio
o
3 -i
3-o
10
4-8
4.6
20
6.9
6-5
25
8.0
7-4
30
95
8.7
Gms. KBrOa per 100 Gms.
Water. Solution.
40 13.2 II-7
50 17-5 J4-9
60 22. f 18.5
80 34-0 25.4
100 50.0 33.3
Sp. Gr. of solution saturated at 19.5° = 1.05.
SOLUBILITY OF POTASSIUM BROMATE IN AQUEOUS SOLUTIONS OP
SODIUM NITRATE AND OF SODIUM CHLORIDE.
(Geffcken — Z. physik. Chem. 49, 296, '04.)
In Sodium Nitrate.
Grams per Liter.
Mols. KBrO3
NaNO3. KBrO3.
per Liter.
o.o 78.79
0.4715
42.54 96.01
0-5745
85.09 108.6
0.6497
170.18 128.3
0.7680
255.27 150.9
0.9026
340.36 172.3
1.031
In Sodium Chloride.
Grams per Liter.
NaCl. KBr03.
o.o 78-79
29 25 82.24
58.50 93.87
117.0 100.9
175-5 IQ4 3
234.0 106.9
Mols. KBrO3
per Liter.
0-47*5
0.5220
0.5616
o . 6042
0.6244
o . 6400
SOLUBILITY OF POTASSIUM BROMATE IN AQUEOUS SOLUTIONS OF VARIOUS
COMPOUNDS AT 25°.
(Rothmund, 1910.)
Solvent, 0.5 Normal T
Aq. Sol. of:
Water alone
Methyl Alcohol
Ethyl' Alcohol
Propyl Alcohol
Tertiary Amyl Alcohol
Acetone
Ethyl Ether
Formaldehyde
Glycol
Glycerol
Mannitol
Grape Sugar
Urea
IBrcfper
Gms.
KBrO3 per
Solvent, 0.5 Normal
Aq Sol of-
Mols.
KBrO3 per
Gms.
KBrOj per
Liter.
Liter.
Liter.
Liter.
0.478
79.84
Dimethylpyrone
0.478
79.84
0-444
74.16
Ammonia
0.445
74-33
0.421
70-33
Dimethylamine
0.384
64.13
0.409
68.31
Pyridine
0.415
69.31
0.383
63.97
Piperidine
0.396
66.15
0.425
70.99
Urethan
0-433
72.33
0-395
65.98
Formamide
0-473
79.02
0-397
66.31
Acetamide
0-445
74-33
0.448
74.84
Glycocol
0.501
83.68
0.451
75-34
Acetic Acid
0.456
76.17
0-451
75-34
Phenol
0.426
7LI5
0.431
71.99
Methylal
0.405
67.66
0-477
79-68
Methyl Acetate
0.420
70.15
POTASSIUM BROMIDE
504
POTASSIUM BROMIDE KBr.
SOLUBILITY IN WATER.
(Average curve from results of Meusser — Z. anorg. Chem. 44, 79, '05; Etard — Compt. rend.
'84; Ann. chim. phys. [7] 2, 526, '94; de Coppet — Ibid. [5] 30,^16, '83; Tilden and
Shenstone — Phil. Trans. 175, 23, '84.)
98, 1432.
Grams KBr per 100 Grams
Grams KBr per 100 Grams
I .
Solution.
Water.
i> .
Solution.
Water.
- 6.5
20. o
25.0
30
41-4
70.6
- 8-5
26.5
35-7
40
43-o
75-5
-10.5
29'5
41.8
50
44-5
80.2
-"•5
31.2
45-3
60
46.1
85-5
— 10
31.8
46.7
70
47-4
QO.O
- 5
33-3
50.0
80
48-7
95-o
o
34-9
53-5
90
49.8
99.2
5
36-1
56.5
IOO
51.0
104.0
10
37-3
59-5
no
52-3
109.5
IS
38-5
62 .5
140
54-7
120.9
20
39-5
65 .2
181
59-3
145.6
25
40.4
67.7
SOLUBILITY OF MIXTURES OP POTASSIUM BROMIDE AND AMMONIUM
BROMIDE IN WATER AT 25°.
(Fock — Z. Kryst. Min. 28, 357, '97-)
rams per Liter Solution. Mol. per cent in S
>olution. Sp. Gr. of
Mol. per cent
in Solid Phas
NH
0
4Br.
• OO
KBr. "
558.1
N
O
.0
KBr. Solutions.
IOO L3756
NHiBr.
o.oo
KBr.
IOO
6
•4
554
.2
I
•38
98
.62 1.3745
O
.26
99-74
24
.64
536
•5
5
.29
94
•71 1-3733
I
•27
98.73
51-34
516.8
10
•77
89
•23
•3721
3
.02
96.98
152
•9
441
.2
29
•63
70
•37
•37^1
8
.42
91.58
262
.2
347
•3
47
.84
52
.16
•3715
17
.20
82.80
347
.6
262
•3
61
.69
38-31
•3753
27
.98
72 .02
381
-4
260
•3
64
•03
35
97 i
•3753
32
•53
67.47
417
.8
232
.2
68
.61
31
39 i
.3766
39
•45
60.55
432
•5
222
•3
70
•27.
29
73 '
•3777
variable
variable
480
.8
179
•9
76
•47
23
53
.3766
98
•53
1.47
577
•3
0
.0
IOO
.0
o
o
•3763
IOO
•o
o.oo
SOLUBILITY OF POTASSIUM BROMIDE AT 25° IN:
Aq. Solutions of KC1 and Vice Versa. Aq. Solutions of KI and Vice Versa.
(Amadori and Pampanini, 1911.)
(Amadori and Pampanini, 1911.)
Cms, per 100 Cms. H2O.
KBr.
KCl/
68.47
0
62.26
5-43
58.50
8.46
52.45
12.48
45-42
17.17
38.70
21.23
26.62
25.88
12.94
31.02
0
36.12
(Seeal
Iso next page.)
Gms. per 100 Cms. H2O.
KBr.
53-21
42.32
34-14
30.08
29.62
22.15
21.88
18-54
o
KI.
35-92
66.63
95-36
119.52
119
127.10
127.31
I30.6I
149.26
505
POTASSIUM BROMIDE
SOLUBILITY OP POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF
POTASSIUM HYDROXIDE.
(Ditte — Compt. rend. 124, 30, '97.)
Grams per 1000 Grams H2O.
' KOH. KB7 '
36-4 558-4
"3-5 433-6
177.2 358.1
231.1 281.2
Grams per 1000 Grams H2O.
KOH. KBr.
277.6 248.1
434-7 J37-i
579.6 64.8
806.9 33.4
SOLUBILITY OF MIXTURES OP POTASSIUM BROMIDE AND CHLORIDE AND
OF MIXTURES OF POTASSIUM BROMIDE AND IODIDE IN WATER.
(Etard — Ann. chim. phys. [7] 3, 275, '97.)
Mixtures of KBr and KC1. Mixtures of KBr and KI.
0 Grams per 100 Gms. Solution.
KBr.
KCl.
— 20
17.5
10.5
0
21-5
10.8
10
23.2
II .0
20
24.8
II .2
25
25-5
"•3
3°
26.3
11.4
40
28.0
"•5
60
30.6
11. 8
80
33-4
12. 1
100
35-7
12 .6
120
38.0
12-9
150
40.6
13-4
Grams per too Grams Solution.
KBr.
9.2
KI.
42-5
9-9
10.2
45-3
46.6
10-5
10-7
10-9
II .2
47-5
48.0
48.6
49.6
II-9
12.6
I3.2
14.0
5*-3
52-7
53-8
54-8
14.9
55-5
SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF
POTASSIUM CHLORIDE, AND OF POTASSIUM CHLORIDE IN AQUEOUS
SOLUTIONS OF POTASSIUM BROMIDE, AT 25.2°.
(Touren — Compt. rend. 130, 1252, 'oo.)
KCl in Aq. KBr Solutions.
KBr in Aq. KCl Solutions.
Mols. per Liter. Grams per Liter.
KCl.
KBr.
KCl.
KBr.
0
.0
4
.76!
0
.0
567
.0
0
.67
4
.22
50
.0
502
•5
0
.81
4
•'5
60
•4
494
.2
I
•35
3
.70
100
•7
440
•7
I
.48
3
•54
no
•4
421
.6
I
.61
3
.42
120
.0
407
.2
I
.70
3
•34
126
.8
397
•7
2
.46
2
•So
183
•5
297
•7
3
•775
O
•525
28l
.6
625
•3
Mols. per Liter.
KBr. KCl.
o.o 4.18
0-49 3-85
0.85 3.58
I-3I 3-19
1.78 2.91
2.25 2.58
2-69 2-33
Grams per Liter.
KBr. KCl.
o.oo 311.8
287.2
267.1
238.0
2I7.I
192.4
173-8
58-4
IOI-3
156.1
211 .9
268.0
320.4
POTASSIUM BROMIDE
506
SOLUBILITY OP POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF
POTASSIUM NITRATE, AND OF POTASSIUM NITRATE IN AQUEOUS
SOLUTIONS OP POTASSIUM BROMIDE, AT 14.5° AND AT 25.2°.
(Touren — Compt. rend. 130, 908, 'oo.)
KNO3 in Aq. KBr Solutions.
KBr in Aqueous KNO3 Solutions.
Mols. per Liter. Grams per Liter.
Mols. per Liter.
Grams per Liter.
KNOs.
Results at
o.o
KBr.
14.2°.
4.332
KNO3.
O-O
KBr.
5*5-9
KBr. KNO3.
Results at 14.20°.
o.o 2.228
KBr.
o.o
KNO3.
225.4
0.362
4.156
36
.6
494
•9
0
.356 2.026
42
•4
205.0
0-706
4-093
71
•4
487
•4
O
.784
•835
93
•4
185-7
1-235
3-939
124
•9
469
.1
I
.092
•730
130
.0
175-0
I
-577
•587
I87
.8
l6o.6
Results at
25.2°.
2
•542
.406
302
•7
142.2
0-0
4.761
O
• o
566
.2
3
•536
•308
421
.i
132.3
O.I3I
4-72
13
•3
561
O
Results at
25.2°.
0.527
4.61
53-3
549
.1
O
.0 3.217
0
.0
325-5
0.721
4-54
72
•9
540
.8
0
.38 3.026
45
•3
306.2
1.09
4-475
no
•3
533
.0
0.93 2.689
no
.8
272.0
I.I70
4-44
118
•4
528
.8
I
•37 2.492
163
.1
252.2
I.C04
4-375
152
.2
521
.1
I
.208 2.216
143
.8
224-3
2
.87 1.958
34i
.8
198.1
3
•55 1-807
422
.8
182.8
SOLUBILITY OP POTASSIUM BROMIDE IN ALCOHOLS AT 25°.
(de Bruyn — Z. physik. Chem. 10, 783, '92; Rohland — Z.. anorg. Chem. 18, 327, '98.)
Grams KBr Dissolved by 100 Gms. Alcohol at:
/iiconoi.
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Room Temp. (R.).
I .92
0.28 (Sp. Gr.
0-055
0.81)
25° (de B.).
i .51 Abs. Alcohol
o.i3
SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS ALCOHOL.
(Taylor — j. Physic. Ch. I, 724, '9<5-'97.)
Results at 30°.
Results at 40°.
Wt. per cent Alcohol
Gms. KBr per
100 Gms.
Gms. KBr per
TOO Gms.
in Solution.
Sat. Solution.
Solvent.
Sat. Solution.
Solvent.
0
41 .62
71.30
43-40
76.65
5
38.98
67.25
40.85
72.70
10
36.33
63.40
38.37
69.00
20
31.09
56.40
33-27
62.30
30
25.98
50-I5
28.32
56-45
40
21 .24
44-95
23.22
50.46
50
16.27
38-85
i8.ii
44-25
60
11.50
32-50
13.02
37-40
70
6.90
24.70
7 -98
28.90
80
3-09
15-95
3-65
18.95
90
0.87
8.80
1.03
10.45
100 gm. acetone dissolve 0.023 gm- KBr at 25°.
(Krug and McElroy — J. anal. Chem. 6, 184, '93.)
507
POTASSIUM BROMIDE
SOLUBILITY OF POTASSIUM BROMIDE IN DILUTE AQUEOUS ETHYL ALCOHOL.
Results at o°.
(Armstrong and Eyre, 1910-11.)
Results at 25°.
(Armstrong, Eyre, Hussey and Paddison, 1907.)
Wt. % CjHBOH
in Solvent.
Gms. KBr per
100 Gms. Sat. Sol.
Wt. % QH6OH
in Solvent.
Gms. KBr per
100 Gms. Sat. Sol.
<f,g of Sat. Sol.
O
34-92
O
40.78
* 1-3824
I.I4
34-35
I.I4
39.98
1.3727
2.25
32.96
2.25
39-54
1.3634
4.41
31-99
4.41
38.41
1-3443
8.44
29-43
12. 14
34-97
1.2815
18-73
30.91
1.2322
100 gms. methyl alcohol dissolve 2.17 gms. KBr at 25°. (Turner and Bissett, 1913.)
ethyl " " 0.142 gm.
propyl
arayl
0-035
0.003
SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF METHYL
ALCOHOL AT 25°.
(Herz and Anders, 1907.)
Wt.% CH3OH Gms. KBr per , nt ~.
in Solvent. 100 cc. Sat. Sol. d*£ of Sat"
VVL. /o v^iij^xa vjrnis. rvur per » » c . Q-I
in Solvent. 100 cc. Sat. Sol. *? of Sat SoL
o 56.04 1-3797 64 10.35 0.9801
10.6 46.28 1.300 78.1 5.24 0.8906
30.8 29.98 . 1.159 98.9 2.74 0.8411
47.1 19.28 1.058 loo 1.69 0.8047
The solubility of potassium bromide in methyl alcohol at the critical tem-
perature is given by Centnerszner (1910), as 0.2 gm. KBr per 100 gms. sat solution.
100 gms. 95% formic acid dissolve 23.2 gms. KBr at 18.5°. (Aschan, 1913.)
loo cc. anhydrous hydrazine dissolve 60 gms. KBr at room temp.
(Welsh and Broderson, 1915.)
loo gms. hydroxylamine dissolve about 44.7 gms. KBr at 17°-! 8°.
(de Bruyn, 1892.)
SOLUBILITY OF POTASSIUM BROMIDE AT 25° IN:
(Herz and Knoch, 1905.)
Aqueous Acetone.
Aqueous
Glycerol.
cc. Acetone
Per 100 cc. Sat. Solution. c 0
wt.%
KBr per 100 cc. Sol. c ^
per loo cc.
Solvent.
Millimols
KBr.
Gms.
KBr.
Gms. Solutions.
H2O.
Glycerol
in Solvent
Millimols.
Gms. Solutions.
O
481.3
57-3
80.6
-3793
O
481.3
57-32 1.3793
2O
366.7
43-67
69-5
.2688
13.28
444-3
52.91
•3704
30
310.5
36.98
62.97
.2118
25.98
404
48.11
.3655
40
259
30.85
55-60
.1558
45-36
340.5
40.55
•3594
50
202.9
24.16
47.60
.0918
54-23
310.4
36.98
.358o
00
144-9
17.22
39.15 1.0275
83-84
219-25
26.11
•3603
70
95-3
11.35
29.78 0.9591
IOO
172.65
20.56 1.3691
80
46.5
5-54
20. 10 0.8942
90
IO.I
i. 20
10.15 0.8340
100 cc. sat. solution of potassium
0.139 gm. KBr at 25°.
bromide in furfurol (C^sO.COH) contain
(Walden, 1906.)
FUSION-POINT DATA FOR MIXTURES OF KBr AND OTHER SALTS.
KBr + KF
KBr + KCi
KBr + KI
KBr + AgBr
KBr + NaCl
KBr + KOH
(Kurnakow and Wrzesnewsky, 1912; Ruff and Plato, 1903.)
(Wrzesnewsky, 1912; Amadori and Pampanini, 1911; Ruff and Plato 1903.)
n « <« « «
(Sandonnini, 1912.)
(Ruff and Plato, 1903.)
(Scarpa, 1915.)
POTASSIUM BUTYRATE
508
POTASSIUM BUTYRATE C3H7COOK.
100 gms. water dissolve 296.8 gms. CsHyCOOK, or 100 gms. sat. solution con-
tain 74.8 gms. at 31.25°.
loo gms. of an aq. solution saturated with sugar and C3H7COOK contain
49.19 gms. sugar + 34.78 gms. C3H7COOK -f 16.03 gms. H2O at 31.25°.
(Kohler, 1897.)
POTASSIUM CAMPHORATES.
SOLUBILITY IN AQUEOUS SOLUTIONS OF d CAMPHORIC ACID AT 13.5-16° AND
VICE VERSA.
(Jungfleisch and Landrieu, 1914.)
Gms. per 100 Gms. Sat. Sol.
Gms. per 100 Gms. Sat. Sol.
CsH14(COOH)2. C10H1404K2.
C8H14(COOH)2.
C10H1404K2.
O 66 . 65 CWH14O4K2
2.90
3 2 . 84 C10H16O4K.CioHi6O4
0 . 90 69 . 69 Ci0H16O4K
3-20
29-39
I 69
3-30
28.56 CjoHuO.K.aQoHuO,
I. io 66.79
3-20
27.32
0.90 66.65 C10HU04K.H2
o 3 . 20
22.77
1.50 62.37
3.10
21.66
2.60 59.34
2.90
12.97
3-20 58-37
2.90
11.73
3-20 58.09
3.10
11.59 dQH^COOH),
3-20 52.71 CioHiAK-QoH
iA 2.90
9.66
3.20 48.43
2.80
8.14
2.80 47.88
2.50
6.76
2.80 42.36
2.30
6.07
3 35-6o
2
4-55
2-85 34-77
0.621
0
CioH14O4K2 = Dipotassium d camphorate.
CioHi6O4K = Monopotassium dtcamphorate.
C10HJ504K.C10H1604 =
Oi0^i5O4.K..3V^lot*l(jO4 —
Monopotassium d dicamphorate.
Monopotassium d tetracamphorate.
POTASSIUM CARBONATE K2CO3.2H2O.
SOLUBILITY IN WATER.
(de Coppet, 1872; Meyerhoffer, 1905; Osaka, 1910-12, Kremann and Zitek, 1909; de Waal, 1910;
Mulder, 1864.)
Gms. K2CO3
t°. per 100 Gms.
Sat. Solution.
— io 21.3
-20 31
-30 36.9
— 36.5 Eutec. 39.6
— 6 . 8 tr. pt. 50 . 9
0 Si-3
-fio 52
20 52.5
25 • 52-8
30 53-2
Solid Phase.
Ice
Gms. K2
per
Sat.
K2CO3.*H2O+K2C03.2H2O
K2CO3.2H2O
40
50
60
70
80
90
100
no
120
130
100 Gms.
Solid Phase.
.. Solution.
53-9
K2CO3.2H20
54-8
"
55-9
d
57-i
«
58.3
«
59-6
H
60.9
u
62.5
«
64.4
«
66.2
11
Single determinations, not in good agreement with the above, are given by
Kohler (1897), by Engel (1888), and by Greenish and Smith (1901).
POTASSIUM BiCARBONATE KHCO3.
SOLUBILITY IN H2O. (Dibbets, 1874.)
t°. o io 20 30 40 60
Gms. KHCO3 per 100 Gms. Sat. Sol. 18.3 21.7 24.9 28.1 31.2 37.5
100 gms. sat. aqueous solution contain 18.7 gms. KHCO3 at o° (d = 1.127)
(Engel, 1888); 23.7 gms KHCO3 at 15° (Greenish & Smith, 1901); 26.3 gms. at
20° (de Forcrand, 1909).
509 POTASSIUM CARBONATE
SOLUBILITY OF POTASSIUM BICARBONATE IN AQUEOUS SOLUTIONS OF
POTASSIUM CARBONATE AT o°. (Engei, 1888.)
Milligram Mols. per i cc. Solution. Sp. Gr. of
Grams per 100 cc. Soluti
iKgCOs.
KHC03 ' Solutions.
' K2CO».
KHCO3.
O-O
21.15
•133
o.o
21.2
17.14
15.28
.182
ii. 8
15-3
24.10
12.65
.20
16.7
12.6
34-50
10.25
.241
23.8
10.3
49-20
7-55
.298
34-o
7.6
62 .14
5.86
•350
43 -o
5-9
74.60
4.90
•398
51.6
4-9
87.50
3-75
.448
60.5
3-8
"7-75
o.o
•542
81.4
o.o
SOLUBILITY OF POTASSIUM CARBONATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AND OF POTASSIUM HYDROXIDE AT 30°. (de Waal, 1910.)
Results for K2CO3 + KC1. Results for K2CO3 + KOH.
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
Solid Phase.
K2C03.
KC1.
OU11U. JTllit&C.
K2C03.
KOH.
53-27
0
K2C03.i*H20
53.27
0
52.22
1.03
" +KC1
2.50
53-77
51-66
1.07
KC1
2.05
55-14
1.64
26.22
"
O
55-75
0
28.01
"
" +KOH.2H2O
• KOH.2H20
loo gms. H2O dissolve 10.76 gms. K2CO3 + 2.66 gms. KNO3 at 10° when both
salts are present in excess. (Kremann and Zitek, 1909.)
IOG gms. H2O dissolve 10.53 gms. K2CO3 + 6.12 gms. Na2CO3 at 10° when
both salts are present in excess (Kremann and Zitek, 1909). See also Potassium
Sodium Carbonate, p. 512.
Data for aqueous solutions of K2CO3 + KNO3 + Na2CO3 + NaNO3, simul-
taneously saturated with two or more of the salts at 10° and at 25°, are also
given by Kremann and Zitek (1909).
Data for the reciprocal salt pairs K2CO3 + BaSO4 <=* K2SO4 + BaCO3 at 25°,
80° and 100° are given by Meyerhoffer (1905).
An aqueous solution, simultaneously saturated with K2CO3.2H2O, K2SO4 and
BaCO3, contains 53.1 gms. K2CO3 + 0.023 gm- K2SO4 at 25°. (Meyerhoffer, 1905.)
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ETHYL ALCOHOL AND
WATER AT 2^0-260. (Frankforter and Frary, 1913-)
NOTE. — The binodal curve for the system (see note, p. 287) was very
carefully determined and tie lines were located by estimations of K2CO3 in spe-
cially prepared conjugated liquids. The original results have been plotted and
the following data for the conjugated layers read from the curve:
Alcohol Rich Layer (Upper) Water Rich Layer (Lower.)
Gms. per 100 Gms. Solution. Gms. per 100 Gms. Solution.
K2C03.
C2H5OH.
H20.
K2C03.
C2H5.
H20.
0.095
90.65
9-255T
53-6
0.28
46.12!
0.241
72.7
27.059
39-n
I
59-89
1.72
53-5
44.78
29.62
4
66.38
4.03
42.6
53-37
25-7
6.4
67.9
6.30
35-5
58.2
21.08
ii
67.92
8.29
31
60.71
I9-I5
13-2
67.65
10-35
27
62.65
18.18
14.7
67.12
14.2
20.5
65.3
14.2
20.5
65.3*
* Plait point.
t Quad, point.
The authors give a complete summary of previous investigations of this system
by de Bruyn (1899, 1900); Bell (1905); Cuno (1908-09).
POTASSIUM CARBONATE 510
Data for the conjugated liquid layers obtained in the system potassium car-
bonate, ethyl alcohol and water at 17° and at 35° are given by de Bruyn (1900)
and at 20°, 40° and 60° by Cuno (1908).
COMPOSITION OF THE CONJUGATED LIQUIDS WHICH ARE IN EQUILIBRIUM WITH
SOLID POTASSIUM CARBONATE (QUADRUPLE POINTS) AT VARIOUS TEMPERATURES.
(de Bruyn, 1900.)
Cms. per 100 Cms. Upper Layer. Cms. per 100 Cms. Lower Layer.
K2CO3. C2HBOH. HA K2CO3. C2H6OH. H^T
— 18 0.03 90.3 9.7 51.2 0.2 48.6
o 0.04 91.9 8.1 51.3 0.2 48.5
+ 17 0.06 91.5 8.4 52.1 0.2 47.7
35 0.07 90.9 9 53.4 0.2 46.4
50 0.09 91.8 8.1 55.3 0.2 44.5
75 °-12 Qi-4 8.5 57.9 0.2 41.9
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, METHYL ALCOHOL,
WATER AT 23°-26°.
(Frankforter and Frary, 1913.)
The authors give the data for the binodal curve and the quadruple points
but tie lines, other than for the quadruple points, were not determined.
Gms. per 100 Grns. Homogeneous Liquid. Cms. per 100 Gms. Homogeneous Liquid.
K2C03.
CH3OH.
H20.
K2C03.
CH3OH.
H20.
6.32
75.85
17.83*
21. 6l
33-43
44.96
6.91
63-I3
29.97
23-15
31.26
45.60
8.07
59.26
32-67
28.25
23-82
47-94
IO.I7
52.64
35-33
30.72
20.57
48.71
12.03
49-97
37-99
32.92
17.27
49.80
14.24
45-74
40.02
40.65
9.26
50.09
16.48
41.76
41.76
43-95
6.96
49.09
18.89
37-76
43-36
45-89
6.42
47.69
49-05
6.1
44-88t
* Upper quad, point. f Lower quad, point.
The following results for the solubility of K2CO3 in concentrations of aq.
CHjOH above and below those yielding liquid layers are also given.
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
CHjOH. K2CO3. fCH3OH. K2CO3.
1-03 51.39 85 2.05
2.22 50.33 89.2 1.56
6.1 49 . 05 (Lower quad, pt.) 91 I • 98
Two Liquid Layers Formed Here. 93-6 2.72
75.85 6.32 (Upper quad pt). 94-3 5-7 (Abs. CH3OH).
Data for the binodal curves for this system at 17° and at 35° are given by
de Bruyn (1900).
m This author also gives the following data for the composition of the conjugated
liquids in equilibrium with solid potassium carbonate (quadruple points) at
various temperatures.
Gms per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer.
CH3OH. H/X
K2C03.
CH3OH.
H20.
-30
21.7
42.2
36.1
— 2O
13-8
52.1
34-1
— 20
12.4
. . .
. . .
0
7.6
66.3
26.1
0
7-4
.
+17
6.2
69^6
24.2
35
5
72.9
22.1
44.2 8.2 47.6
46.3 6.7 47
46.6 6.6 46.8
48.3 5.7 46
51 4.3 44.7
5ii POTASSIUM CARBONATE
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, NORMAL PROPYL
ALCOHOL AND WATER AT 22°-26°.
(Frankforter and Frary, 1913.)
The authors give the data for the binodal curve and the quadruple points
but tie lines were not located.
Cms. per 100 Cms. Homogeneous Liquid. Cms. per 100 Cms. Homogeneous Liquid.
K2C03.
C3H7OH.
H20
K2C03.
CaH7OH.
HA
52.9
46.98
O.O2
0.12
47-08*
52-91
7-45
5-97
9-30
11.07
83-25
82.96
39
0.20
60.80
4-73
12.71
82.56
34-58
0.20
65-I5
3-86
14.60
81.54
3° -43
0-45
69.12
3-n
17.17
79.71
26.51
0.78
72.71
2.42
24.71
72.87
22.81
1.32
75-87
1.91
34-90
63.19
19.08
2-31
78.62
1.71
39
59-29
16.35
3-24
80.41
i-33
45-57
53-09
13-47
4.41
82.12
0.948
51-56
47-49
10.99
6.24
82.77
0.387
64.20
35-41
8-55
8-31
83-14
0.017
95-83
4-i53t
Lower quad, point. t Upper quad, point.
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ISOPROPYL ALCOHOL
AND WATER AT 20°.
(Frankforter and Temple, 1915.)
NOTE. — The results for the binodal curve in this and the following system are
reported in terms of gms. per 100 gms. solvent (water + alcohol) instead of gms.
per 100 gms. of homogeneous liquid (K2COa + water + alcohol.)
Gms. per 100 Gms. Alcohol + Water. Gms. per 100 Gms. Alcohol + Water.
K2C03.
Alcohol.
Water.
K2C03.
Alcohol.
Water.
44.844
2.911
97.089
15.021
19-445
80.555
36.137
4.783
95-217
I3-244
23.919
76.081
28.879
7-349
92.651
6.065
45-397
54-603
24.152
9-159
90.841
3-933
53-265
46.735
17.665
14-395
85-605
2-954
57-294
42.706
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ALLYL ALCOHOL AND
WATER AT 20°.
(Frankforter and Temple, 1915.)
Gms. per 100 Gms. Alcohol -{- Water. Gms. per 100 Gms. Alcohol + Water.
K2CO8. Alcohol. Water. K2CO3. Alcohol. Water.
47.746 2.103 97.897 8.239 30-677 69.323
33.200 5.267 94-733 5-521 39-337 60.663
23.486 9-309 90.691 2.020 54-487 45-513
16.354 15-037 84.963 1.015 62.610 37-390
11.331 22.454 77-546 0.0853 81.228 18.772
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ACETONE, WATER AT 20°.
(See also Acetone, p. 1 3) . (Frankforter and Cohen, 1914.)
The binodal curve was very carefully determined and, in addition, data for the
quadruple points (solid K2CO3) and five tie lines were located. These data were
plotted and the following interpolated values for the conjugated liquids read
from the curve.
Gms. per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer.
K2C03.
(CH3)2CO.
H20.
K2CO3. (CH3)2CO.
H20.
0.0024
96.4
3-5+t
52.4 trace
47- 6f
0.039
64
35-96
32-63 1.2
66.17
0.712
55-3
43-99
24-4 3-7
71.9
1.36
48.5
50.14
22.91 4.7
72-39
4-57
34
61.43
16.92 10.2
72.88
6-97
27-5
6S-53
14-77 13
72.23
10.5
20
69-5*
10.5 20
69.5
* Plait point.
t Quad, points.
POTASSIUM CARBONATE
512
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, POTASSIUM DIPROPYL
MALONATE AND WATER AT 25°.
(M 'David, 1909-10.)
A series of mixtures of K2CO3 + KCuHwOi + H2O were prepared and thoroughly
mixed. They were placed in a thermostat at 25° and the two layers which sep-
arated in each case, were analyzed.
Cms. per 100 Gms. Upper Layer. Cms. per 100 Cms. Lower Layer.
K2C03.
KCUH1904.
H20.
4-05
65-1
30-85
4-9
59-8
35-3
5-6
53-5
40.9
7.2
.50-5
42.3
8-7
39-2
S2.i
ii
34-6
54-4
14-5
23-5
62
17
18.6
64-4
18.6
15
66.4
K2C03.
KCUH1904.
H20.
42.6
0.4
57
40-7
0.4
58-9
35
0-5
64.5
33-5
0.9
65-6
28.9
0.7
70.4
26.8
0.8
72.4
24.8
• 3
72.2
23-1
6.05
70.8-
21.7
8-7
69.6'
Several determinations at 2° and at 56° are also given.
100 cc. anhydrous hydrazine dissolve I gm. K2CO3 at room temp.
(Welsh and Broderson, 1915.)
loo gms. aqueous solution simultaneously sat. with K2CO3 and cane sugar at
31.25° contain 22.24 gms- K2CO3 and 56 gms. sugar. (Ktihler, 1897.)
Freezing-point data for mixtures of K2CO3 + KC1 and K2CO3 + NaCl (Sackur,
1911-12). K2CO3 + K2SO4 (Amadori, 1912; Le Chatelier, 1894); K2CO3
+Na2CO3 (Le Chatelier, 1894). (Le Chatelier, 1894.)
POTASSIUM Sodium CARBONATE K2CO3.Na2CO3.i2H2O.
SOLUBILITY IN WATER AT 25°.
(Osaka, 1910-11.)
Gms. per 100 Gms. Sat. Sol.
Gms. per 100 Gms. Sat. Sol.
K2C03.
Na2C03. '
K2C03.
Na,C03.
52.83
o K2CO3.2H2O
25.2
14.1
52
I "
22.4
16.6
50.7
2.6
19.8
18.7
. 49-1
4.6 " -f-KzCOa.NajCOa.isHzO
19.1
19.7
49
4 . 6 K2CO3.Na2CO3.i 2H2O
23.2
46.5
4-3 "
14.5
22.8
46.2
5- 2
10.8
22.7
41
6-3
10.7
22.4
37-7
7
4-7
21.9
31
10.5
o
22.71
Solid Phase.
+Na2CO3.ioH2O
Na2C03.ioH2O
The previous determinations of Kremann and Zitek (1909), agree in general
with the above, but these authors report that the double salt contains 6H2O
instead of I2H2O.
100 gms. H2O dissolve 184 gms. potassium sodium carbonate at 15° (d = 1.366).
(Stolba, 1865.)
POTASSIUM URANYL CARBONATE 2K2CO3.(UO2)CO3.
loo gms. H2O dissolve 7.4 gms. salt at 15°. (Ebelmen, 1852.)
POTASSIUM CHLORATE KC1O3.
SOLUBILITY IN WATER.
Average curve from results of Carlson (1910), Calzolari (1912), and Tschugueff and Chlopin (1914).
O
10
15
20
25
30
d of Sat. Sol.
Gms. KC1O3 per
100 Gms. H2O.
I.O2I
3-3
L
1.045
7-4
8.8
10.5
40
£
80
100
104 b. pt.
d of Sat. Sol.
Gms. KC1O3 per
100 Gms. H20.
1.073
14
19-3
1.115
1.165
24-5
38.5
1.219
1.230
57
60
For previous results in good agreement with the above, see next page.
513
POTASSIUM CHLORATE
POTASSIUM CHLORATE KC1O3. (See also previous page.)
SOLUBILITY IN WATER.
(Gay-Lussac, 1819; Pawlewski, 1899; above 100°, Tilden and Shenstone, i88i;'see also Blarez,
1891; Etard, 1894; at 99°, Kohler, 1879.)
Gms. KClOg per 100 Gms.
O
10
20
25
30
40
50
60
Solution.
w
ater.
3-04
3-i4
3-3*
4.27
4-45
5 -°
6.76
7.22
7.1
7-56
8.17
8.6
8.46
9.26
10. 1
ii .75
I3-31
14-5
15.18
17-95
19.7
18.97
23.42
26.0
t°.
Gms. KC1O3 per 100 Cms.
Solution.
Water.
70 22-55
80 26.97
90 3I-36
loo 35-83
I2O 42.4
136 49-7
190 64.6
330 96.7
* Gay Lussac.
ioo gms. H2O dissolve 5.06 gms. KC1O3 at 10°.
One liter of H2O dissolves 65.5 gms. KCJO3 at about 20'
29.16 32.5*
46.11
55-54
73-7
98-5
183.0
2930-00
39-6
47-5
56.0
73-7
99.0
183.0
(Roozeboom, 1891.)
_ (Konowalow, iSggb.)
One liter of 5.2 % NH3 solution dissolves 52.5 gms. KC1O3 at about 20°. "
SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF POTASSIUM
HYDROXIDE, HYDROGEN PEROXIDE, AND MIXTURES OF THE Two AT 25°.
(Calvert, 1901.)
The mixtures were agitated by means of a stream of air. Equilibrium was
approached both from above and below 25°.
Mols. KClOj Gms. KC1O3
Dissolved per Dissolved per
Liter of Sat. Sol. Liter of Sat. Sol.
Composition of Solvent.
Water alone
Aqueous o. 125 n KOH
0.25 n "
Aq. H2O2 containing i . 26 mols. H2O2 per 1.
1.31
Aq. 0.25 n KOH ' 0.015
0.276
0-954
1.073
SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF
0.675
82.71
0.625
76.60
0.573
70.23
erl.
0.730
89-45
«
0.737
90.33
«
0.578
70.82
«
6.584
71-57
1C
0.616
75-50
((
0.673
82.47
POTASSIUM
Gms. per ioo Gms.
Solution.
BROMIDE AT 13°.
Gms. per ioo Gms.
Solution.
(Blarez, i
Gms.
per ioo Gms.
Solution.
'KBr.
0.20
0.60
0.8
KC103. "
5.18
5.20
5-06
'KBr.
1-0
2.0
3-o
4-0
KC1O3.
5-04
4.60
4-2
4-0
KBr.
6.0
8.0
IO-O
KC1CV
3-46
2.8o
2.40
SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF OTHER
POTASSIUM SALTS AT 14°-! 5°. (Blarez,
K Salt.
KC103.
oaii. f
K Salt.
KC103.
KOH
1-43
4-47
KNO3
2-59
4-51
KC1
1.91
4-45
M
5-i8
3-88
"
3-82
3-58
K^SO,
2.23
4-7i
KBr
3-05
4.49
M
4.46
"
6.10
3.60
K2C2O4
2.42
4.72
KI
4-25
4-59
"
4-85
3-93
"
8.51
3-65
POTASSIUM CHLORATE 514
SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF
POTASSIUM CHLORIDE AT 20°.
(Winteler — Z. Electrochem. 79 360, 'oo.>
Sp. Gr. of
Grams per Liter.
Sp. Gr. of
Grams
F>er Liter.
Solutions.
KC1. KC103.
Solutions.
KC1.
KC103:
1.050
o 71.1
1.098
120
24-5
1.050
10 58.0
I.IOS
140
22.5
1.050
20 49-0
I .119
160
21.0
1.054
40 39-5
I.I30
180
20. o
I .064
60 34.0
I.I40
200
2O *}
1-075
80 30.0
I.I68
250
20. o
1. 086
ioo 27.0
SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OP
POTASSIUM NITRATE.
(Arrhenius — Z. physik. Chem. n, 397, '93.)
Results at 19.85'
Mols. per Liter.
Grams per Liter.
Results at 23.87°.
Mols. rjer Liter. Grams per Liter.
KNO3.
KC103."
'KN03.
KC103" " KN03. KC1O3"
KN03.
KC103.
O
• O
0
570
O
.O
69.
88 o.o 0.645
O
• o
79
.09
O
•125
o.
529
12
•65
64-
86 0.5 0.515
50
•59
63
.14
O
•25
o
492
25
.29
60.
33
I
.0
o
•374
IOI
.19
45-
85
2
.0
0
•328
2O2
•38
40.
22
SOLUBILITY OF POTASSIUM CHLORATE:
(Taylor, 1897; see also Gerardin, 1865.)
In Aqueous Alcohol.
In Aqueous Acetone.
Wt. per cent „ At3°-
Alcohol or Gms. KC103per
of Acetone ioo Gms.
At 40°.
Gms. KClOg per
ioo Gms.
At 30°.
Gms. KC1O3 per
ioo Gms.
At 40°.
Gms. KC1O3 per
ioo Gms.
insolvent. Soiution
. Water.
Solution.
Water.
Solution.
Water.
Solution.
Water.
O
9-23
IO
•17
12.23
J3-93
9
•23
10
•17
12.23
13-93
5
7-7«
8
.80
10.48
12 -33
8
•32
9
•56
II .10
I3.II
10
6.44
7
•65
8.84
10.77
7
.63*
9
.09
10.28*
12 .60
20
4-51
5
.90
6.40
8.56
6
.09
8
.10
8.27
II .26
30
3-21
4
•74
4.67
7.00
4
•93
7
.40
6.69
10.24
40
2-35
4
.00
3-41
5-88
3
.90
6
.76
5-36
9-45
50
i .64
3
•33
2-41
4-94
2
.90
5
.98
4-03
8.40
60
I .01
2
•53
I.4I
3-69
2
•03
c
•17
2.86
7-35
70
0-54
I
.82
0.78
2.63
I
.24
4
.18
1.68
5.68
80
0.24
I
.22
o-34
J-73
O
•57
2
.88
o-79
3-97
90
0-06
0
.62
O-I2
1.17
0
.18
I
,82
0.24
2-45
* Solvent, 9.09 Wt. per cent Acetone.
ioo gms. sat. solution of KC1O3 in glycol contain 0.9 gms. KC1O3.
(de Coninck, 1905.)
515
POTASSIUM CHLORATE
SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF VARIOUS
COMPOUNDS AT 25°. (Rothmund, 1910.)
Aqueous 0.5 Normal
Solution of:
Water alone
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Tertiary Amyl Alcohol
Acetone
Ether
Glycol
Glycerol
Urea
100 gms. glycerol (du = 1 .256) dissolve 3.54 gms. KC1O3 at 15-16°. (Ossendowski, 1907.)
POTASSIUM PerCHLORATE KC1O4.
SOLUBILITY IN WATER.
(Average curve from results of Noyes and Sammet (1903); Carlson (1910); Rosenheim and Weinhaber
(1910-11); Calzolari (1912); Thin and Gumming (1915).
KC1O3 per Liter.
Aqueous 0.5 Normal
KC1O3 per Liter.
Mols.
Gms.
Solution of:
Mols.
Gms.
O.
1475
20.
44
Ammonia
O.
1474
2O
•43
Q-
1402
19.
43
Dimethylamine
0.
1342
18
.66
0.
1356
18.
75
Pyridine
0.
1410
19
•54
0.
1343
18.
61
Urethan
O.
1400
19
.40
0.
1279
17-
72
Formamide
0.
J539
21.32
0.
1451
20.
ii
Acetamide
0.
1447
20
•05
0.
1336
18.
51
Acetic Acid
O.
1462
2O
.26
0.
1416
19.
62
Phenol
0.
1362
18
.87
0.
1404
19.
45
Methylal
0.
1400
19
.40
0.
1510
20.
92
Methyl Acetate
0.
1429
19
.80
O
10
2O
25
30
40
doi
Sat. Sol.
1.007
Gms. KC1O4 per
ioo Gms. H2O.
0-75
<f of
Gms. KC1O4 per
t .
Sat. Sol.
ioo Gms. Sat. Sol.
50
6-5
60
1-033
9
70
. . .
ii. 8
80
1-053
14.8
90
. . .
18
IOO
1.067
21.8
01 Oil I. 80
1. 012 2.08
2.6
1.022 4.4
SOLUBILITY OF POTASSIUM PERCHLORATE IN AQUEOUS AND IN ALCOHOLIC
SOLUTIONS OF PERCHLORIC ACID AT 25.2°.
(Thin and Gumming, 1915.)
In Alcoholic HC1O4 Solutions.
Aqueous Solvent. x^S^S&g
2.085 93.5% Alcohol 0.051
1.999 " +o.2%HC104* o.OI75
o.io 1.485 98.8% Alcohol + o.oio
i 0.527 " +2%HC1O4* 0.028
In Aq. HC1O4 Solutions.
Normality of Aq. Gms. KC1O4
HC1O4. loo Gms. Sat.
o (= water)
o.oi
The HC1O4 was added as aq. 20% HC1O4 solution hence the concentration of the alcohol was decreased.
SOLUBILITY OF POTASSIUM PERCHLORATE IN AQ. KC1 AND AQ. K2SO4
SOLUTIONS AT 25°. (Noyes and Boggs, 1911.)
In Aq. KC1 Solutions.
Grns^per 100.2 cc. Sat. Sol. wt. of 100.2 cc.
of Solution.
101.42
101.45
In Aq. K2SO4 Solutions.
Gms. per 100.2 cc. Sat. Sol. \yt. of 100.2 cc.
KC1O4. K2SO4. of Solution.
2.0566 o
1.8262 0.4339 101.47
1.6396 0.8665 101-55
KC1O4. KC1.
2 .0566 O
1.7800 0.3715
x-5597 0.7421
ioo gms. 51.2 Vol. % Aq. C2H6OH (d =0.9319) dissolve 0.754 gpi. KC1O4 at 25.2°.
(Thin and Gumming, 1915.)
93-5 (^=0.8219) 0.051 gm. KC1O4 at 25.2°.
(Thin and Gumming, 1915.)
98.8 (^ = 0.7998) " 0.019 gm. KC1O4 at 25.2°.
(Thin and Gumming, 1915.)
90 Wt. % Aq. C2H6OH " 0.036 gm. KC1O4 at 25.2°.
4« «
97.2
(Wenze, 1891.)
0.0156 gm. KC1O4 at 25.2°.
(Wenze, 1891.)
POTASSIUM CHLORIDE 516
POTASSIUM CHLORIDE KC1.
SOLUBILITY IN WATER.
(Average curve from the results of Meusser — Z. anorg. Chem. 44, 79, '05; at 31.25°, Kohler — Z.
Ver. Zuckerind. 47, 447, '07; Andrae — J. pr. Chem. [2] 29, 456, '84; Gerardin — Ann. chim. phys.
[4] St i37. '65; de Coppet Ibid. [5] 30, 411, '83; Etard Ibid. [7] 2,526, '94; Mulder; above 100°, Tilden
and Shenstone — Proc. Roy. Soc. (Lond.) 35. 345. '83-)
to
Gms. KC1 per 100 Gms.
X0 Gms. KCl per ioo Gms.
t°
Gms. KCl per ioo
Gms.
Solution.
Water.
Solution.
Water.
Solution.
Water.
-9
19
•3
23
•9
40
28.6
40
.0
147
41-5
70.8
-4'
5 20
.6
25
•9
50
29.9
42
.6
180
43-7
77-5
0
21
.6
27
.6
60
3J-3
45
q
Solid Phase
Ice
5
22
•7
29
•3
70
32.6
48
3
-9
19-3
23-9
10
23
•7
31
.0
80
33-8
51
i
-8
• 17-7
21 -5
15
24
•5
32
•4
90
35 -,1
54
.0
-8
16.7
20.0
20
25
•4
34
.0
IOO
36.2
56
•7
-7
14.9
!7-5
25
26
.2
35
•5
130
39-8
66
.0
-6
13.6
15-7
30
27
.1
37
.0
-5
•5 I2-5
14-3
Sp. Gr. of solution sat. at o = °i.i5o; at 15° = 1.172.
The following determinations of the solubility of potassium chloride in water,
made with exceptional care, are reported by Berkeley (1904).
*o d of Gms. KCl per ioo « d of Gms. KCl per ioo
Sat. Sol. Gms. H2O. t ' Sat. Sol. Gms. H2O.
0.70 I.I540 28.29 74.80 1.2032 49.58
19.55 1-1738 34-37 89.45 1.2069 53-38
32.80 1.1839 38-32 108 (b. pt.) 1.2118 58.11
59.85 1.1980 45.84
IOO gms. H2O dissolve 36.12 gms. KCl at 25°. (Amadoriand Pampanini, 1911.)
F.-pt. data for aq. KCl solutions are given by Roloff (1895).
Data for equilibrium in the system potassium chloride, arsenic trioxide and
water at 30° are given by Schreinemakers and de Baat (1915).
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
CHLORIC ACID AT 0° AND AT 25°.
(Armstrong, Eyre, Hussey and Paddinson, 1907; Armstrong and Eyre, 1910-11.)
Solvent, Gms. KCl per ioo Gms. Sat. Sol.
Gms. HClper , *- >
1000 Gms. H2O. At o°. At 25°.
O 22.11 26.45
9.11 20.93 25-J7
18.22 I9-7I 24.07
36.45 17.26 21.74
109-35 •'• 13-47
182.25 ••• 6-93
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
BROMIC ACID AND OF HYDROCHLORIC ACID AT 25°. (Herz, 1911-12.)
In Aq. HBr. In Aq. HC1.
Millimols per 10 cc. Gms. per Liter. Millimols j>er 10 cc. Gms. per Liter.
HBr. KCl. HBr. KCl. HC1. KCl. ' HC1. KCl.'
o 42.72 o 318.5 5.66 37.49 20.64 279.6
6.61 37.80 53.5 281.9 I0-20 33-79 37-*9 252
34.15 19-57 276.4 146 15.91 28.68 57.98 213.9
20.94 24.74 76.35 146.6
32.52 17.39 Il8-6 129.6.
517
POTASSIUM CHLORIDE
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS
HYDROCHLORIC ACID AT o°.
(Jeannel — Compt. rend. 103, 381, '86; Engel — Ann. chim. phys. [6] 13, 377, '88.)
OF
ram Mols
per 10 cc.
Grams per ipo cc. Solution. gD- Qr> of
KC1.
HCI:
KCl.
HCI. Solutions.
34-5
o.o
25-73
0-0
•159
30.41
3-9
22 .69
1.42
•152
27-95
6.6
20.84
2.41
.150
27-5
7-i
20.51
2.59 ]
.147
23-75
ii .1
17.71
4-05 ]
•137
16.0
23.0
n-93
8-39
.in
lo.o
34-o
7.46
12.40 3
.105
7-5
41 .0
5.60
*4-95
.105
2.0
65-5
1.49
23.88
.121
2-4
148.8 (sat.)
1.52
54.26
.224
100 cc. saturated HCI solution dissolve 1.9 gms. KC1 at 17°. „ (Ditte, 1881.)
100 gms. sat. aq. HCI solution dissolve 1.9 gms. KC1 at 20°. (Stoltzenberg, 1912.)
F.-pt. data for mixtures of KC1 and HCI are given by Dernby (1918).
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND OF SODIUM CHLORIDE
IN AQUEOUS HYDROCHLORIC ACID SOLUTIONS AT 25°.
(Hicks, 1915.)
Gms. per 100 Gms. Sat. Solutions.
HCI.
NaCl.
KCl.
0
19-95
10.90
8.61
10.65
7-58
17.16
3-56
3.80
20.65
2.03
2.86
32.78
0.18
1.27
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS MAGNESIUM
CHLORIDE SOLUTIONS.
(Precht and Wittgen — Ber. 14, 1667, '81.)
Grams KCl per 100 Grams Sat. Solution in:
t°.
II
Mg(
% 15%
:i2. MKci2.
21.2%
MgCb.
3°%
MKC12.
20% MgCl2.
10
14
•3
9
9
5-3
I
•9
4
.2KCl+5.7NaC
20
15
•9
ii
,3
6-5
2
.6
6
.0
1 +5-9
tt
30
17
•5
12
•7
7.6
3
•4
6
•9
" +6.0
tt
40
19
.0
14
.2
8.8
4
.2
7
•9
" +6.1
n
50
20
•5
15
.6
IO-O
5
.0
8
•9
" +6-3
tt
60
21
•9
17
• o
II. 2
5
.8
9
•9
" +6.4
tt
80
24
•5
J9
•5
13-6
7
•3
10
•9
" +6.6
tf
90
25
.8
20
.8
14.7
8
.1
ii
•9
" +6.7
t(
100
27
.1
22
.1
J5-9
8
•9
13
.0
" +6.9
u
More recent data on the solubility of potassium chloride in aqueous solutions
of magnesium chloride are given by Feit and Przibylla (1909).
POTASSIUM CHLORIDE 518
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM
BROMIDE AT 25°.
(Fock, 1897.)
Grams per Litef
Solution.
Milligram Mols.
per Liter.
M°kcfinCent Sp.Gr.of
r- i • Solutions
Mol. per cent
KCI in
KBr.
KCI:
KBr.
KCI.
Solution.
Solid Phase.
558
.1
0
.00
4686.2
O
.0
o
o
I
•3756
o.oo
.5
23
•44
4462.7
3*4
.2
6
.16
I
.3700
o.oo
503
.6
46
•57
4228.5
624.3
12
.86
I
•3648
8.23
454
.6
82
.62
3817.8
1108
• O
22
•49
I
•3544
15.68
379
.6
136
.6
3I88.I
1830
•7
36
.48
I
•3320
33-66
324
.8
166
•9
2727.6
2237
•4
45
.06
I
•3IJ9
63-51
218
.0
213
•9
1830.2
2868
.0
60
•30
I
.2689
82.29
140
•7
250
•9
1181.1
3363
•9
74
.01
I
•2455
88.04
47
•5
291
•7
398.8
39"
•4
85
.22
I
.1977
96.98
o
.0
311
•3
0-0
.1
IOO
• OO
I
•1756
100.00
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS POTASSIUM
HYDROXIDE SOLUTIONS.
(Engel — Bull. soc. chim. [3] 6, 16, '91; Winteler — Z. Electrochem. 7, 360, 'oo.)
Results at
0°.
Results at 20°.
(Engel.)
(Winteler.)
Mg. Mols. per
10 cc. Solution S>P-
Gr. of
Jution.
Gms. per 100 cc.
Solution.
Gms. per 100 cc.
Solution. £
p. Gr. of
olution.
KCI.
KOH.
KCI.
KOH.
KCI. KOH. '
35-5
o 1.159
26.83
o.o
29.3 i.o
.185
31.0
2.375 1.146
23-44
J-33
21. I IO.O
• 2IO
28.3
4-7 1-153
21.39
2.64
14.8 20. o
-245
23.0
9.9 1.172
17-39
5-56
IO-4 30.0
•295
18.38
15 1
•195
13.89
8.46
6.8 40 . o
•345
14-43
20. o
.216
10.91
11.23
4-0 50.0
•397
n-43
24.63
•239
8.64
13-83
2.2 60 • O
•450
8.98
29.25
.261
6.78
16.43
1-4 70.0
.500
6.28
35-*3
.294
4-74
19.72
I.I 80 . O
•550
0-9 85.0
.580
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM
IODIDE IN WATER.
(Etard — Ann. chim. phys. [7] 3, 275, '94.)
Grams per TOO Gms. Solution
Grams per 100 Gms. Solution.
* •
KCI.
Kl.
i .
KCI.
KI.
o
3-7
50-5
IOO
6.2
61 .0
20
4.2
53-o
140
7-3
63-7
40
4-7
55-3
180
8-3
65-5
60
5-2
57-5
220
9-4
66-3
80
5-7
59-4
245
IO.O
66.5
519
POTASSIUM CHLORIDE
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
IODIDE AT 25° AND VICE VERSA.
(Amadori and Pampanini, 1911.)
Gms. per 100 Cms. H2O.
KC1.
KI.
0
149 . 26
4.06
144.03
7-63
137-79
11.36
132.60
11.74
I33-90
15.10
105.91
Gms. per 100 Gms. H2O.
KC1.
KI. '
19.64
68.22
23-75
43-89
29.56
23-83
31.38
14.83
33-68 '
7
36.12
o
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
NITRATE AT o° AND AT 25°.
(Armstrong and Eyre, 1910-11.)
Solvent, Gms. KNO3
per 1000 Gms.
H20.
O
25.27
50-55
IOI.II
151.66
Gms. KC1 Dissolved per
zoo Gms. Sat. Solution at:
o .
22. IO
21.71
21.25
20.70
25 •
26.73
26.26
25.61
24.58
23-57
SOLUBILITY DATA FOR THE RECIPROCAL SALT PAIRS KCl+NaNO3^NaCl+KNO3
AT 5°, 25°, 50° AND IOO°.
(Reinders, 1914, 1915; see also Uyeda, 1909-10.)
Results at 25°.
Gms. per 100 Gms. H20.
Results at 50°.
Gms. per 100 Gms. H2O.
Solid Phase in Each
Case.
NaCl
NaCl+KCl
KC1
KC1+KN03
i KNO3
KN03+NaN03
NaNO,
NaNOj+NaCl
NaCl
NaCl+KCl
KCl+KNOs
KNO3+NaNO3
NaNO3+NaCl -
NaCl+NaNO2+KN03
NaCl+KCl+KNO3
NaCl. KC1.
36 . 04
32.28 10
30.27 16.45
12 26.78
35-54
34.92
IO
IO
23.62
33-90
24.82 22.2
21.36 2O
24-5
23.8 :::
4-5
NaNO3.
10
60
100.9
96.06
77.46
58.01
IO
15-4
61.3
82.1
64
KNO3.
IO
22.79
31.48
37-49
41.87
46.15
20
32-9
17.2
43-15
41.2
40-3
NaCl.
36.72
28 .'35
KC1. NaNO3.
23.09 ...
42 . 80
41-39 ..-
38.75 .-.
KN03.
24.05
52.54
85.10
20.5
28.4
34
12.7
... 134.9
... 114.1
... 84.8
... 43-9
13-4
25-4
90.2
24-3
58.6
19.2
12.2
59-9
104 . i
110.7
6.1
27.2
82.2
70.9
31-50
27.6
Results at 5*.
10.4
29.84
82.10
41.7
10.14
18.1
27.3
19.2
Results at iooc
36-2
41 .6
233-6
158
199
218
NaCl+KCl
KC1+KN03
KN03+NaNO3
NaNO3+NaCl
POTASSIUM CHLORIDE
520
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
NITRATE, AND OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE, AT SEVERAL TEMPERATURES.
(Touren, 1900; Bodlander, 1891; Nicol, 1891; Soch, 1898.)
KC1 in Aq. KNO3 Solutions at:
14-5° (T.).
25.2° (T.).
20°, etc. (N.).
Gms. per Liter Solution.
Gms. per Liter Solution.
Gms. per 1000 Gms. HgO.
KN03. KC1.
' KNO3. KC1.
KNO3. KC1.
o 288.3
o 311.8
o 345-2
20 . 64 284 . 2
13.76 306.6
56.18 342.15
32.18 282.1
32.18 303.6
168.54 334-39
62.23 276.8
91.26 293.2
at 25° (S)
82.77 273.5
122.7 287.2
225.8 341.3
II5.9 270.7
I4I.4 284.2
at 80° (S)
II9.I 268.3
182.7 276
1175 402
123.4 267.2
KN03 in Aq. KC1 Solutions at:
14-5°.
25.2°.
20°.
Gms. per Liter Solution.
Gms. per Liter Solution.
Gms. per 1000 Gms. H2O.
KC1. KNO,.
KC1. KNO3.
KC1. KNO3.
o 225.4
o 325.5
o 311.1
13.58 219.8
19.39 312.3
82.9 256.8
31.63 208.2
49-22 288.7
165.8 221.7
65.64 185.2
100.7 254
248 . 7 202
132.6 159.5
155.2 224.4
310.8 501.6
164.4 153-3
207.3 203.9
196.5 144
226.8 196.9
236.9 I37.I
In the case of the results by Touren, constant temperature and agitation were
employed.
KN03 in Aq. KC1 at
20.5° (B.). KC1 in Aq.
KN03 at 17.5° (B.).
Gms. per 100 cc. Solution.
Sp. Gr. of Gms. per 100 cc
Solution. • Sp. Gr. of
' KC1. KN03. '
Solutions. " KNO3.
KC1. Solutions.
o 27 68
.1625 o
29.39 1-173°
4.72 24.39
.1700 6.58
27.50 , 1.1980
7-74 22.44
.1765 8.88
27.34 I. 2100
12.23 20.23
.1895 12.48
26.53 1.2250
15.15 18.96
.1983 14.83
25.98 1.2360
I9.6l 17-67
.2150 15.22
25.96 1.2300
22.17 17.11
.2265 15-49
25.95 1-2388
24.96 16.79
.2400 15.33
26.24 I.24IO
In the case of the above results by Bodlander, a saturated aqueous solution of
potassium chloride was prepared and weighed amounts of potassium nitrate were
added to measured volumes of it. The mixtures were warmed and then allowed
to cool to the indicated temperature and frequently shaken during 24 hours.
521
POTASSIUM CHLORIDE
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
NITRATE AND VICE VERSA.
(Leather and Mukerji, 1913.)
Results at 30°.
Sp. Gr.
Sat. Sol.
1.186
1.219
1.251
1.281
1.258
1.241
1.225
Cms. per 100 Cms.
KCl.
37.58
36.72
36.19
35-42
28.71
19.35
9-44
H20.
KN03.
O
8.05
19.36
26.83
29.19
32.34
38.10
Results at 40°.
Gms. per too Gms. ,
H?O. j
p.Gr.
at. Sol.
.222
•344
.486
•552
•544
•545
.552
Results at 91°.
Gms. per 100 Gms.
H20.
Solid Phase
in
Each Case.
KCl
" +KNO,
KNO,
KCl.
40.60
39.11
37.08
3749
32.22
22.63
11.58
KN03." "
0
16.86
35-45
39-71
41.52
46.31
52.66
KCl.
53.58
47.85
43-30
39-90
33.25
J5-56
0
KNO?."
0
52.75
114.6
162.9
165.6
181.1
202.8
Sp. Gr.
Sat. Sol.
I.I94
1.252
I.305
I.3I9
I.3I2
1.297
1.279
Results are also given for 20°.
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND SODIUM
CHLORIDE IN WATER.
Gms. per 100 Gms. H2O.
Gms. per 100 Gms. H2O.
KCl.
NaCl.
KCl.
NaCl.
O
II
.2(l) 11.2(2) 30(1)
30(2)
50
22(1)
19(2)
27.7(l)
32.3(2)
IO
12
•5
12.3
29-7
30.5
60
24
.6
20.6
27.2
32.8
20
14
.7
13.8
29.2
31
70
27
•3
32.5
26.8
34.1
25
17
) 14.5
29(3)
31.3
80
31
(3)
25.2(3)
26.4(3)
34
30
17
.2
15.4
28.7
31-5
90
32
•9
28.4
26.1
32.3
40
19
•5
17
28.2
31-9
100
34
•7
32.3
25-8
30.6
(i) Precht and Wittgen, 1881; (2) Etard, 1897; (3) at 25° and at 80°, Soch, 1898.
NOTE. — Page and Keightly, Rudorff and also Nicol give single determinations
which lie nearer the results of Precht and Wittgen than to those of Etard.
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AND VICE VERSA.
(Leather and Mukerji, 1913; see also Nicol, 1891.)
Sp. Gr.
>at. Sol.
.176
.197
.213
•237
.240
•233
.224
•193
Results at 20°.
Gms. per 100 Gms. (
H2O. ^
>p. Gr.
at. Sol.
.194
.207
•235
.248
.242
[.247
.222
.197
Results at 40°
Gms. per 100 Gms.
H20.
Sp. Gr.
1.222
1.236
1.262
1.262
1.264
1-235
1.223
1.189
Results at 91°.
Gms. per 100 Gms.
H20.
Solid Phase
in
Each Case.
KCl
it
" +NaCl
NaCl
KCl.
34.6l
26.60
19.65
14.92
I5.36
14.76
9.70
O
NaCl.
O
10.13
20.61
30.36
29.61
30.38
32.40
35.63
KCl.
40.60
31.42
2443
18.23
18.74
19.13
10.49
NaCl. '
0
10.68
20.99
30.60
30.32
29.92
32.59
36.53
KCl.
45.01
35.84
33.12
32.45
27.15
13
O
NaCl.
O
10.66
22.87
28.12
28.26
29.18
33-93
38.72
Results are also given for 30°.
100 gms. 40 wt. per cent alcohol dissolve 5.87 gms. KCl + 12.25 gms. NaCl at 25°.
loo gms. 40 wt.'per cent alcohol dissolve 5.29 gms. KNO3 + 10.06 gms. KCl at 25°.
(Soch, 1898.)
100 gms. abs. ethyl alcohol dissolve 0.034 gm. KCl at 18.5°.
100 gms. abs. methyl alcohol dissolve 0.5 gm. KCl at 18.5°.
(de Bruyn, 1892; Rohland, 1898.)
POTASSIUM CHLORIDE 522
SOLUBILITY DATA FOR THE RECIPROCAL SALT PAIRS KCl+Na2SO4^K2SO4+NaCl.
(Meyerhoffer and Saunders, 1899.)
, ftf Mols. per 1000 Mols. H2O.
t°. <Vf f *- > Solid Phase.
Sat. Sol. S04. K2. Na,. C12.
4.4* ... 5.42 14-39 Si-83 60.8 K3Na(S04)2+KCl+NaCl
0.2 ... 3.35 12.78 50.93 60.36 Na4SO4.ioHrf)-fKCl+NaCl
— 0.4 ... 3.59 16.38 40.75 53.54 NaaSO4.ioH40+KCl+K,Na(SO4)«
16 ... 4.72 17.58 50.56 63.42 K3Na(SO4)2+KCl+NaCl
24.8 1.2484 4.37 20.02 48.36 64.01
16 . 3* ... 16 . 29 9.16 61 . 06 53 . 93 KsNa(SO4)2+NaCl+Na2SO4.ioH2O+Na2S04
24.5 1.2625 14.45 9-QO 58.46 53-91 K3Na(SO4)2+NaCl+Na2SO4
0.3 ... 2.75 25.77 17.93 40.95 K3Na(S04)2+KCl+K2SO4
25 1.2034 2.94 36.20 14.80 48.06
17.9* 1.2470 13.84 O 62.54 48.70 Na2SO4.ioH2O+Na2SO4+NaCl
30.1* 1.289 50.41 10.08 40.33 o K3Na(SO4)2+Na2SO4.ioH2O+Na2SO4
* tr. pt.
Curves are given in the original paper and a complete discussion of the older work.
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM
SULFATE IN WATER.
Gms. per 100 Cms. H2O. . 0 Gms. per too Gms. H2O.
^ ' KCl + K.SO.. ' °bSErVer' '• KC1 + K,SO..
IO 30 . 9 1.32 (Precht & Wittgen.) 40 38-7 I . 68 (P. and W.)
15.8 28 2.3 (Kopp.) 50 41.3 1.82
20 33.4 1.43 (P.andW.) 60 43.8 1. 94
25 34 .76 2.93 (Van't Hoff & Meyerhoffer.) 80 49-2 2.21 "
30 36.1 1.57 (P.andW.) 100 54.5 2.53
100 gms. aq. solution, sat. with both salts, contain 26.2 gms. KCl + 1.09 gms.
K2SO4 at 30°. (Schreinemakers and de Baat, 1914.)
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS 'OF STANNOUS
CHLORIDE AT 25° AND VICE VERSA. (Fujimura, 1914-)
Gms. per 100 Gms. H2O. Gms. per 100 Gms. H2O.
Solid Phase. — ' Sohd Phase.
KCl.
O 34-73 KC1 58.48 17.85 SnCl2.KCl.H20
2.86 32.17 " 81.78 19.06
4.37 34.08 " 107.65 17.79
5-95 3I-76 SnCi2.2KCi.2H2o 170.70 21.26
5.83 30.65 " 247.50 24.38
10.24 27.30 337-26 25-5x
17.42 24.68 " 290.30 19.66 SnCl2.2H2O
27.88 24.40 " 235.50 7.49
34-28 5.99 222.5 2-73
54.19 19.45 SnCl2.KCl.H20 234.05
SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE SOLUTIONS OF ETHYL
ALCOHOL AT o° AND AT 25°.
(Armstrong, Eyre, Hussey and Paddison, 1907; Armstrong and Eyre, 1910-11.)
Wt. % Gms. KCl Dissolved per 100 Gms.
QHsOH Sat. Sol. at: <%of
in , * s Sol. Sat.
Solvent. o°. 25°.
O 22.1 26.44 I.l8l3
1.14 21.6 25.91 I.I754
2.25 20.9 25.29 1.1689
4.41 19.7 24.21 1.1568
8.44 ... 22.46 LI357
12.13 15-5
18.69 ••• I7-42 1.0847
523
POTASSIUM CHLORIDE
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS ALCOHOL.
(Gerardin — Ann. chim. phys. [4] 5, 140, '65.)
Interpolated from the original results.
Grams KC1 per too Gms. Aq. Alcohol of Sp. Gr.:
t".
0.9904
0.9848
0.9793
0.9726
0.9573
0-939
0.8967
0.8244
Wt.5*.
wt'f.
= 13-6
Wt.%.
= 19.1
Wt.%.
= 30
Wt.%.
= 40
Wt.%.
= 60
Wt.%.
= 90
Wt. %.
o
23-4
iQ-5
I5-S
"•S
7.0
4.0
i-7
o.o
5
25.0
21.0
16.8
12.8
8.0
4.8
2.2
0-0
10
26.4
22.5
18.0
14.0
9.0
5-6
2-7
0-0
15
26.8
24.0
19.2
15-2
IO.O
6.4
3-i
0.04
20
29.1
25-3
20.3
16. i
10.8
7.2
3-5
0.06
25
30-4
26.8
2i-S
17.1
ii. 6
7-9
3-9
0.08
30
3!-7
28.0
22.6
18.2
12.5
8-5
4.2
o.io
40
34-3
30.8
24.8
20-0
14.0
9-9
4.8
O.2O
50
37-o
33-5
27.0
21.8
*5-5
10.8
5-2
0.30
60
16.8
ii.8
5-5
0-40
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS ALCOHOL AT:
(Schiff — Liebig's Ann. 118, 365, *6i.)
14-5 •
(Bodlander — Z. physik. Ch. 7, 316, '91.)
Sp. Gr.
Wt.
G. KC1 per
Sp. Gr.
of Sat
Grams per 100 cc. Solution.
Alcohol.
per cent
Alcohol.
100 jr. AQ.
Alcohol.
oi oat.
Solutions.
CjjHsOH.
H20.
KCI:
0.984
10
19
.8
I
.1720
. .
88
.10
29.10
0.972
2O
14
•7
I
.1542
2
•79
85
.78
26
•85
0.958
30
10
•7
I
•J365
4
.98
84
.00
24
.67
0.940
40
7
•7
I
•1075
10
•56
79
•63
20
•56
0-918
So
5
.0
I
.1085
15
•57
75
.24
17
.24
0.896
60
2
.8
I
•0545
20
.66
70
•S2
14
.27
0.848
80
O
•45
I
•0455
24
•25
67
•05
13
•25
Gerardin 's results
at 15° agree
0
•9695
40
.42
5o
.18
6
•35
well with
the above
deter-
0
•9315
48
•73
40
.60
3
.82
minations
.
O
.8448
68
•63
15
•55
o
•30
30° and 40°.
(Bathrick — J. Physic. Chem. i, 160, '96.)
Wt.
per cent
Alcohol.
Gms. KCI per 100 Gms.
Aq.jUcohol.
Wt.
per cent
Alcohol.
Gms. KCI per too Gnc
Aq. Alcohol.
At 30°.
At 40°.
"At 30°.
At 40°."
O
38.9
41.8
43.1
II. I
13.1
5-28
33-9
35-9
55-9
6.8
8.2
9-43
30.2
33-3
65-9
3-6
4.1
16.9
24.9
27.6
78.1
1.6
25-1
19.2
21.8
86.2
0.4
0-5
15-6
17.2
POTASSIUM CHLORIDE
524
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF ETHYL
ALCOHOL AT 25°.
(Mclntosh, 1903.)
vt. %
HsOH,
Mols. KC1
per Liter.
Gms. KC1 per
ioo cc. Sat. Sol.
Wt. %
QHsOH.
Mols. KC1
per Liter.
Gms. KC1 per
ioo cc. Sat. Sol.
0
4.18
3I.I8
60
0.56
4.18
10
3-21
23-93
70
0-305
2.27
20
2.40
17.89
80
0.125
o-93
3°
1.78
I3-27
90
O.O42
0.31
40
1.26
9.40
IOO
O.OII
0.08
50
0.84
6.26
SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE AQUEOUS SOLUTIONS OF
METHYL ALCOHOL AT o° AND AT 25°.
(Armstrong and Eyre, 1910-11.)
Wt. %
PN OH
Gms. KC1 per ioo Gms. Sat. Sol. at;
v^Xl^UXl
in Solvent.
o°.
25°.
0
22.06
26.69
0.79
21.74
26.42
i-57
21.39
26.OI
3.10
20. 6l
25-25
8.76
17.84
22.82
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS METHYL ALCOHOL AT 25°.
(Herz and Anders, 1907; Mclntosh, 1903.)
Solvent
flfog Of
Gms
.KCl
Solve
:nt.
j
oc Of
Gms. KCl
,, wt. %
d«F CH3OH.
Sat. Sol.
per ioo cc.
Sat. Sol. dap-
Wt.%
CH3OH
Satfsol
per ioo cc.
Sat. Sol.
O,
,9971
0
1.1782
31
.13
0
.8820
64
o.
9064
3-44
o
,9791
10.6
I.I25
24
.53
0
.8489
78.1
0.
8607
1-54
0
,9481
30.8
1.033
13
-65
0
.8167
98. 9(?
) o.
8242
0-75
o.
.9180
47.1
0.9679
7
.6l
o
.7882
IOO
o.
7937
0-43
ioo gms.
methyl
alcohol dissolve
0-53
gm. KCl
at 25°.
(Turner and Bissett, 1913.)
ti
ethyl
11
11
0.022
« «
it
««
"
n
propyl
«
«
0.004
« «
M
«
"
amyl " 0.0008
Potassium chloride is insoluble in CHsOH at the crit. temp. (Centnerszwer, 1910.)
SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE AQUEOUS SOLUTIONS OF
PROPYL ALCOHOL AT o° AND AT 25°.
(Armstrong and Eyre, 1910-11.)
Wt. %
C3H7OH
in Solvent.
I
1.48
2.91
5.66
Gms. KC1 per 100 Gms. Sat. Sol. at:
o°.
22.O6
21.25
20.49
18.97
25°.
26.44
25.94
25.23
23.82
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF GLUCOSE AT 25°.
(Armstrong and Eyre, 1910-11.)
wt.%
Gms. KCl
C6H1206+H,O
per ioo Gms.
in Aq. Solvent.
Sat. Solution.
0
26.63
4.72
25.86
9
25.18
16.53
23.89
37-27
20.15
525
POTASSIUM CHLORIDE
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS ACETONE SOLUTIONS.
(Snell, 1898; at 20°, Herz and Knoch, 1904.)
Wt. (see Note) _At 20 .
Percent KClperioocc.
Acetone in Solution.
At 30°.
Gms. per 100 Gms.
Solution.
At 40°.
Gms. per 100 Gms.
Solution.
At 50°.
Gms. per 100 Gms.
Solution.
Solvent.
Millimols.
Gms.
Acetone.
KCl.
Acetone. KCl. '
Acetone. KCl. "
0
410.5
30.
62
0
27-
27
O
28.69
0
30
Q.I
351-7
26.
23
6.
96
23-
42
6.
79 25.33
... •
. . .
20
286.6
21 .
38
16.
22
18.
90
15-
75 21.28
. . .
. . .
30
223.7
16.
69
25-
45
15-
06
two layers
25.67
14.42
40
166.5
12.
42
35-
52
II .
31
it
36.03
9-93
50
II5-4
8.
61
45-
98
8.
04
t(
46.46
7.07
60
71.2
5-
31
56-
9i
5-
12
a
57-37
4-38
70
38-5
2.
87
68.
18
2.
60
(i
68.56
2.22
80
I2.Q
O.
96
79-
43
0.
76
79
34 0.58
79-25
0.94
90
2
0.
15
89.
88
O.
13
89
.84 0.16
±81°
sat. sol.
100
O
0
100
0
100
0
NOTE. — For the 20° results the per cent acetone in the solvent is in terms
of volume instead of weight per cent, and the concentration of the second solu-
tion is 10 per cent instead of 9.1 which is the weight per cent concentration of the
solvent for the corresponding results at the other temperatures.
AT THE TEMPERATURE 40° AND FOR CONCENTRATIONS OF ACETONE BETWEEN 20
AND 8O PER CENT THE SATURATED SOLUTION SEPARATES INTO TWO LAYERS
HAVING THE FOLLOWING COMPOSITIONS:
Upper Layer.
Gms. per 100 Gms. Solution.
H20.
(CH3)2CO.
KCl.
55-2
31.82
12.99
53-27
35-44
11.29
51-23
48.50
10.27
50-34
39-88
9-77
48.02
43-i8
8.79
46.49
45-34
8.17
58.99
25.24
15-77
Lower Layer.
Gms. per 100 Gms. Solution.
rH20.
(CH3)2CO.
KCl.
28.14
69.42
2.44
30.96
65-97
3-07
32.64
63-79
3-56
34-07
62.01
3-92
37-44
57-67
4.89
38.68
56.17
5-25
23.66
74.91
i-43
100 cc. sat. solution of potassium chloride in furfurol (C^aO.COH) contain
0.085 gm. KCl at 25°. (Walden, 1906.)
POTASSIUM CHLORIDE 526
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF GLYCEROL AT 25°.
(Herz and Knoch, 1905.)
Sp. Gr. of Glycerol at 25°/4° = 1.2555. Impurity about 1.5%.
Wt. Per cent
Glycerol in
Solvent.
KCl per ioo cc.
Solution.
Sp. Gr. of
Solutions.
Wt. Per cent
Glycerol in
Solvent.
KCl per ioo cc.
Solution.
Sp. Gr. of
Solutions.
Millimols.
Gms.
Millimols.
Gms.
0
424.5
31.66
I
.180
54
23
238.
5
17
79
I .219
13.28
383.4
28.61
I
.185
83
.84
149
II
.11
1.259
25.98
339-3
25-3I
I
.194
IOO
no
.6
8
25
1.286
45.36
271.4
20.24
I
.211
100 gms. H2O dissolve 246.5 gms. sugar + 44.8 gms. KCl at 31.25°, or 100 gms.
of the sat. solution contain 62.28 gms. sugar + H-33 gms. KCl. (Kohler, 1897.)
SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF PYRIDINE AT 10°.
(Schroeder, 1908.)
Aq. Mixture. Gms. KCl Aq. Mixture. Gms. KCl
, • — per 100 Gms. ' — » per too Gms.
cc. H2O. cc. Pyridine. Sat. Sol. cc- H2O. cc. Pyndine. Sat. Sol.
ioo o 23.79 40 60 3.33
90 10 19-76 30 70 1.25
80 20 16.37 20 80 0.24
70 30 I3-I9 1° 90 0-04
60 40 * 10.05 o ioo o
50 50 6-34
SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE AQUEOUS SOLUTIONS OF
SEVERAL COMPOUNDS AT 25°.
(Armstrong and Eyre, 1913.)
Gms. Cmpd. Gms. KCl Gms. Cmpd. Gms. KCl
Compound. per 1000 Gms. per ioo Gms. Compound, per 1000 Gms. per ioo Gms.
H2O. Sat. Sol. H2O. Sat. Sol.
Water alone ... 26.89 Glycol I5-5* 26.43
Acetaldehyde n.oi 27.05 62.05 25.26
Paraldehyde n.oi 26.42 Mannitol 45-53 24.86
Glycerol 13.01 25.58 136-59 24.46
ioo gms. 95% formic acid dissolve 19.4 gms. KCl at 19. 7°. (Aschan, 1913.)
glycerol (di6 = 1.256) 3.72 ' " 15-16°. (Ossendowski, 1907.)
ioo cc. anhydrous hydrazine " 9 " " " room temp.
(Welsh and Broderson, 1915.)
ioo gms. hydroxylamine 12.3 " 17-18°. (de Bruyn, 1892.)
FUSION-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES OF POTASSIUM CHLORIDE AND OTHER SALTS.
vr'ij^irT \ (Wrzesnewski/ia; Amadori&Pam- vr'l-Lircr* I (Jaenecke, '12; Sackur, '11-12;
«"KL i panmi,'n; Ruff & Plato, '03.) KUHK2bU4.j Ruff & plato/03>)
KC1 + KF. (Ruff and Plato, 1903.) KCl + HgCl (Sackur, 1913.)
KC1 + KOH. (Scarpa, 1915.) KCl + NaCl. (Sackur, '13; Ruff & Plato, 03.)
KCl-i-KCrO4. (Sackur,'ii-i2;Zemcznzny,'o8.) KCl-i-Na2SO4. (Sackur, 1913.)
KCl + KPOs. (Amadori, 1912.) KCl+SrCl2. (Vortisch, '14; Sackur, '11-12.)
KC1+K4P2O7. " KC1+T1C1. (Sandonnini, J9"J 1914-)
KC1+K3PO4.
POTASSIUM CHLOROIRIDATE K2IrCl6.
ioo gms. H2O dissolve 1.25 gms. of the salt at 18-20°.
ioo gms. H2O dissolve 9.18 gms. dipotassium aquopentachloroiridite, IrCl6
(H2O)K2 at 19°. (Delepine, 1908.)
527
POTASSIUM CHROMATES
POTASSIUM CHROMATES K2CrO4, K2Cr2O7, K2Cr3Oi0> etc.
EQUILIBRIUM IN THE SYSTEM, POTASSIUM OXIDE, CHROMIC ACID AND
WATER AT SEVERAL TEMPERATURES.
(Koppel and Blumenthal, 1907.)
Results at o°. Results at 30°.
Results at 60°.
Gms. per 100 Gms. Sat.
Solution.
Gms.
per too Gms.
' Solution.
Sat.
Gms.
per too Gms. Sat.
Solution.
Solid Phase at each
' K20.
Cr03. '
K20.
Cr03.
' KA
Cr203.
Temp.
3I.I8
.
46.
8
about 50
KOH.2H2O
26.06
0
•54
26.
89
0.
94
32
.98
o.
53
K2Cr04
19.31
4
•27
22.
25
3-
06
21
.05
9-
15
"
17.06
ii
•77
18.
65
13-
72
20
•25
14.
43
"
17.62
18
.71
19.
12
20.
30
20
.70
21 .
97
"
17-73
19
.04
19.
35
21
2O
.61
23-
61
" +K2CrA
10.90
ii
•93
15-
04
16.
85
14-53
20.
82
K2CrA
1.87
3
•13
II.
20
13-
ii
IO
.OI
21 .
21
"
0.78
22
-38
2.
42
28.
21
6
.86
39-
64
"
i-47
42
•95
2.
50
44.
50
7
.06
49-
84
" +K2CrAo
1.25
44
-52
4
.06
54-
73
K2CrAo
1.17
46
.84
.
.
2
60.
69
"
i-37
47
.40
2.
35
49-
95
. .
. .
" +K2Cr4Oi3
1.24
48.23
I.
35
53-
39
.
. .
. .
.
K2Cr4O13
1.16
56
•93
. .
.
. .
.
.
. .
"
0.64
61
•79
0.
69
62.
81
I
.27
65-
77
" +Cr03
0
61
•54
.
62.
52
0
65-
12
CrO,
THE CRYOHYDRATES (EUTECTICS) IN THE SYSTEM K2O — CrO3 — H2O.
The points were determined by adding to a sat. solution of K2Cr2O7 successive
I to 2 gm. portions of. chromic acid and ascertaining the freezing-point and
composition of the solution. At the point of appearance of a new solid phase an
additional amount of chromic acid does not change the f.-pt. since the added CrOa
goes into the solid phase. This relation also holds at the points where the solu-
tion is simultaneously saturated with K2Cr2O7 and K2Cr2Oio or K2Cr2Oi0 and
K2Cr4013.
t° of Equi-
librium of
Sat Sol
Gms. per 100 Gms. Solid Phase
Sat. Solution. inj£uffitaraiii
t° of Equi-
librium of
Cj, * Cnl
Gms. per 100 Gms.
Sat. Solution.
Solid Phase
in Equilibrium
with Sat. Sol.
with Ice.
K2O.
CrO3. and jce>
oat. ooi.
with Ice.
' K2O.
CrO3.
and Ice.
-25
2O
5
. 70 K2CrO4
— 13
.22
not det.
27
.26
K2CrA
17
.52
13
.89 "
-14
•50
u
28
•85
"
— II
•37
17
.12
18
.18 «*
— 22
.IO
ft
35
.92
"
— II
•50
17
.18
18
.11 " +K2CrA
— 22
.11
0.47
36
.14
"
-5
8
•27
8
. OI K2CrA
-26
•77
0.88
39
.86
M
— o.
63
i
•38
2
•93 " *
-30
.20
1.18
42
.31
~l~K2Cr3Ojo
— i .
78
not
det.
6
.81
-34
.01
0-95
43
•45
K2CrA0
-5-
5
tt
16
.05 "
-39
0.79
45
•65
" +K2CrA,
-6.
43
0
•48
17
.25
-49
not det.
49
.11
K2Cr4013
IO.
25
o
•45
23
•63
-61
•5
0.61
53
•57
*
The viscosity of the solutions at the lower temperatures increased so much that
the cryohydrate points could not be determined. By graphic extrapolation the
cryohydrate temperature of chromic acid and of chromic acid + potassium tetra-
chromate is near —80° and the CrO3 content is 59 gms. per 100 gms. sat. solution.
POTASSIUM CHROMATES
528
By interpolation from the data given in the preceding tables the following
solubilities in water are obtained :
THE ICE CURVE AND SOLUBILITY OF POTASSIUM CHROMATE IN WATER.
to Gms. K2CrO4 per Solid
100 Gms. H2O. Phase.
- o-99 4-53 Ice
—1.2 6.12 "
- 4.3. 26.99
— 7.12 42.04
-10.35 52.41
Potassium Potassii
Dichromate + Potasi
Gms. K2Cr2O7 I
t°. per 100 Gms. t°.
H20.
-0.63* 4.50 -II.5*
o 4.65 o
30 I8.I3 +30
60 45.44 60
104. 8f 108.2 io6.8t
*•• *£&£%& SoHd Phase.
-11.35 EuteC. 54 . 54 Ice+K2CrO4
O 57 .11 K2CrO4
30 65 . 13
60 74.60
io5.8b.pt. 88.8
im Dichromate Potassium Dichromate
sium Chromate. + Potassium Trichromate.
Gms. per 100 Gms. H2O. f0 Gms' p£^ms' Sat
K2O. CrO3.
17.18 i8.ii
17.73 19.03
19-35 21
20. 61 23.61
24-3 30.5
-30*
0
+ 20
3°
60
K20.
1.18
1.47
2.20
2.50
7.06
16.80
Cr03.
42.51
42.99
43.10
44-50
49.84
59.20
Eutec.
Potassium Trichromate + Potassium
Tetrachromate.
*
' K20.
Cr03.
—39 Eutec.
0.79
45-69
0
i-37
47.40
20
2
48.46
30
2.25
49-95
60
5.01
54-09
t b. pt.
Potassium Tetrachromate-f-
Chromic Acid (CrOs).
Gms. per 100 Gms. Sat. Sol.
O
20
30
60
K20.
0.64
O.62
0.69
1.27
Cr03.
61.79
62.80
62.81
Data for boiling points in the system K2O + CrO3.H2O determined by means
of the Beckmann apparatus, are also given.
The older data for K2CrO4 and K2Cr2O7 are as follows:
SOLUBILITY OF EACH IN WATER.
(Alluard, 1864; Nordenskjold and Lindstrom, 1869; Etard, 1894; Kremers, 1854; Tilden and Shen-
stone, 1884.)
Potassium Dichromate.
Potassium Chromate.
Grams per 100 Grams Water.
Grams per 100 Grams Water.
0
58.2*
59 -3t
60.2*
10
60-0
61.2
62.5
20
61.7
63.*
64-5
25
62.5
64.2
64-5
30
63-4
65.2
66.5
40
65.2
67.0
68.6
50
66.8
69.0
70.6
60
68.6
71.0
72.7
70
70.4
73-o
74.8
80
72.1
75-o
76.9
90
73-9
77-o
79-o
100
75-6
79-o
82.2
"5
79-o
150
83.0
5*
5§
7
7
12
12
16
16
20
20
26
27
34
37
43
47
52
58
61
70
70
82
80
97
no
145
*43
205
* Etard.
t Alluard.
N. and L.
§ A., K., T. and S.
529
POTASSIUM CHROMATES
SOLUBILITY OF POTASSIUM CHROMATES IN WATER AT 30*
(Schreinemaker — Z. physik, Ch. 55, 83, '06.)
Composition in Wt. per cent of:
Solid
The Solution
Per cent CrO3 Per cent K2O .
The Residue.
Per cent CrO3. Per cent K2O .
0
±47
. . .
o.o
47.16
12.59
47-54
0.1775
34.602
10-93
37-47
I-351
26.602
16.482
32.532
20.584
37-I3I
39.922
15-407
19.225
27.966
29-377
20.67
19.17
19.096
17.30
37.64
22.61
7.88
. . .
. . .
17-93
3.412
25-85
7.82
43 -51
3-oi
49-45
9.91
44.46
3-245
53-94
12.40
46.368
2.823
60.314
12.935
49-357
2-353
63-044
11.684
53-215
1.360
62.958
8.002
62-55
0.796
67.944
6.731
62.997
0.621
70.0
4.0
62.28
Q.O
. . .
. . .
Phase.
KOH-zHzO
K2Cr207
K2Cr3O10
K2Cr40,3
K2Cr4Ol3 + Cr08
Cr03
IOO gms. sat. solution in glycol, C?H4(OH)2.H2O, contain 1.7 gms. K2CrO4at 15.4°.
IOO gms. sat. solution in glycol, C2H4(OH)2.H2O, contain 6 gms. K2Cr2O7 at 14.6°.
(de Coninck, 1905.)
IOO gms. H2O dissolve IO.I gms. K2Cr2O7 at 15.5°. (Greenish and Smith, 1901.)
ioo gms. sat. solution in water contain 5.52 gms. K2Cr2O7 at 4.81°, 15.17 gms.
at 30.1° and 1777 gms. at 35.33°. (Le Blanc and Schmandt, 1911.)
ioo cc. sat. aqueous solution contain 11.43 gms. K2Cr2O7 at 20°.
(Sherrill and Eaton, 1907.)
SOLUBILITY OF POTASSIUM CHROMATE IN AQUEOUS SOLUTIONS OF POTASSIUM
MOLYBDATE AT 25° AND VlCE VERSA.
(Amadori, 191 aa.)
Gms. per ioo Gms. H2O.
K2Cr04.
64-62
49-59
38.90
33-21
K2Mo04.
O
15-37
38.79
50.96
Gms. per ioo Gms. H2O.
'K2CrO4. K2MoO4.
14.13 98.72
10.07 118.8
10.24 119.9
7.12 137.8
6.37 157.2
Gms. per ioo Gms. H2O.
K2Cr04. K2MoO4.
4.92 165.4
2.14 I80.8
1.70 183
o 184.6
SOLUBILITY OF POTASSIUM CHROMATE IN AQUEOUS SOLUTIONS OF
POTASSIUM SULFATE AT 25° AND VICE VERSA.
(Amadori, 191 2a.)
Gms. per ioo Gms. H2O.
K2CrO7 K2SO4. '
63.09 0.76
61.39 I.I7
58.40 1.84
5I.8I 2.36
Gms. per ioo Gms. H2O.
K2CrO4.
40.93
27.36
20.83
14.65
K2S04.
3.33
4.82
5-72
7.12
Gms. per ioo Gms. H2O.
K2Cr04.
7.8l
4.36
1.94
O
K2S04.
8.98
IO.25
10.86
12. IO
IOO cc. anhydrous hydrazine dissolve I gm. K2CrO4 at room temp. ) (Welsh and Brod-
100 cc. anhydrous hydrazine dissolve i gm. K2Cr2O7 at room temp. J erson, 1915.)
POTASSIUM CHROMATES 530
FREEZING-POINT DATA (Solubilities, see footnote, p. i) FOR MIXTURES OF
POTASSIUM CHROMATES AND OTHER COMPOUNDS.
K2CrO4 + K2Cr2O7. (Groschuff, 1908.)
' K2CrO4 -j- K2MoO4. (Amadori, 1913.)
K2CraO7 -j- K2Mo2O7.
K2CrO4 -j- K2SO4. (Amadori, 1913; Groschuff, 1908.)
K2CrO4 + K2WO4. (Amadori, 1913.)
K2Cr2O7 + K2W2O7.
POTASSIUM CITRATE (CH2)2C(OH)(COOK)3.H2O.
SOLUBILITY IN WATER.
(Average results of Seidell, 1910; Greenish and Smith, 1901; Kohler, 1897.)
Gms. (CH2)2C(OH)(COOK)3.H2O per ioo Gms.
Sat. Solution. Water.
15 6l.8 l62
20 63.2 172
25 64.5 l82 (^25 = L5l8)
30 66 194
ioo gms. H2O dissolve 198.3 gms. (CH2)2COH(COOK)3 + 303.9 gms. cane
sugar at 31.25°- (Kohler, 1897.)
SOLUBILITY OF POTASSIUM CITRATE IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
When potassium citrate is added to aqueous alcohol of certain concentrations
the mixture separates into two liquid layers. A series of determinations made by
adding an excess of the salt to 10-15 cc. portions of several aq. alcohol mixtures
at 25° gave the following results.
Wt.%
. C2HBOH
in Solvent.
d«5 of
Sat. Solution.
' Wt. %_
C^HsOH in
Sat. Solution.
Gms. (CH2)2COH-
(COOK)3.H2O
per ioo Gms.
Sat. Solution.
8.9
(a
lb
1.4920
O
60
(a
. . .
...
0.2
32
lb
1.4930
0
6l.6
iff
(a
. . .
65.1
0.38
S1
lb
62.5
*7O "?
(a
0.8366
81
O.IO
7O.2
lb
...
62.3
8l.4
0/8356
8l.4
0.038
91.6
0.8139
91 .6
0.016
99-9
0.7896
99-5
0.014
a = upper, alcohol rich layer, b = lower, water rich layer.
A series of determinations was also made by adding just enough potassium
citrate to the alcohol solution to cause distinct clouding and then, after bringing
to 25°, titrating with the aqueous alcohol mixture to disappearance of the clouding.
The results were plotted and the following interpolated values obtained.
Wt.%
in Solvent.
Gms. (CH2)2COH-
<*u of (COOK)3.H20
Sat. Solution. per ioo Gms.
Sat. Sol.
wt.%
CzHsOH
in Solvent.
Gms.(CH2)2COH-
duol (COOK)3H20,
Sat. Solution, per ioo Gms.
Sat. Sol.
0
I.5l8
64.5
40
I .005
12.4
5
1.400
52-5
50
0-943
5-6
10
I.3IO
45-5
60
0.900
1.6
20
I.I77
31-5
70
0.868
0.4
3° „
1.085
21.5
80
0.838
0.04
In one determination at 15°, made with alcohol of 59 Vol. per cent, 4.51 gms.
(CH2)2COH(COOK)s.H2O were required to just cause clouding.
531 POTASSIUM CYANATE
POTASSIUM CYANATE KCNO.
SOLUBILITY IN ALCOHOLIC MIXTURES.
(Erdmann, 1893.)
Cms. KCNO
Solvent. per Liter Solvent
at b.-pt.
80 per cent Alcohol + 20 per cent Water 62
80 per cent Alcohol + 20 per cent Methyl Alcohol 76
80 per cent Alcohol + 10 per cent Acetone 82
POTASSIUM CYANIDE KCN.
100 gms. H2O dissolve 122.2 gms. KCN, or 100 gms. sat. solution contain 55
gms. KCN at 103.3°. (Griffiths.)
100 gms. abs. ethyl alcohol dissolve 0.87 gm. KCN at 19.5°.
100 gms. abs. methyl alcohol dissolve 4.91 gms. KCN at 19.5°. (de Bruyn, 1892.)
100 gms. glycerol dissolve 32 gms. KCN at 15.5°. (Ossendowski, 1907.)
100 gms. hydroxylamine dissolve 41 gms. KCN at 17.5°. (de Bruyn, 1892.)
F.-pt. data for KCN + KC1, KCN + NaCN, KCN + AgCN, KCN + Cu2
(CN)2 and for KCN + Zn(CN)2 are given by Truthe (1912).
POTASSIUM CHROMOCYANIDE K3Cr(CN)6.
100 gms. H2O dissolve 32.33 gms. K3Cr(CN)e at 20°.
(Moissan, 1885; Christensen, 1885.)
POTASSIUM CHROMITHIOCYANATE K2Cr(SCN)6.4H2O.
IOO gms. H2O dissolve 139 gms. salt. (Karsten, 1864-5.)
POTASSIUM CARBONYL FERROCYANIDE K3FeCO(CN)6.3^H2O.
IOO gms. H2O dissolve 148" gms. salt at 16°. (Muller, 1887.)
POTASSIUM FERRICYANIDE KsFe(CN)8.
POTASSIUM FERROCYANIDE K4Fe(CN)6.3H,O.
SOLUBILITY OF EACH IN WATER.
(Wallace, 1855; Etard, 1894; Schiff, 1860; Michel and Krafft, 1858; Thomsen.)
NOTE. — The available determinations fall very irregularly when plotted on
cross-section paper, and the following figures, which are averages, are therefore
hardly more than rough approximations to the true amounts. The figures under
K4Fe(CN)6 show the limits between which the correct values probably lie.
Gms. per 100 Gms. H2O.
Gms. per 100 Gms. H2O.
0
10
2O
25
10
K3Fe(CN)6.
31
36
43
46
<o
K4Fe(CN),.'
13 •••
2O 2O
25 40
28 48
^2 <J7
40
60
80
IOO
IO4.4.
K3Fe(CN)6.
60
66
82.6
K4Fe(CN),.'
38 70
52 83
66 89
76 91
loo gms. H2O dissolve 0.08946 gm. mols. = 32.97'gms. K4Fe(CN)6 at 25°, da^ of
sat. sol. = 1.0908. (Harkins and Pearce, 1916.)
One liter of sat. solution in water contains 319.4 gms. K4Fe(CN)6.3H2O at 25°.
(Grube, 1914.)
Using the Harkins and Pearce figure for dap, this result corresponds to 34.3 gms.
K4Fe(CN)6 per 100 gms. H2O.
One liter of sat. solution in water contains 385.5 gms. K3Fe(CN)6 at 25°.
(Grube, 1916.)
POTASSIUM FERRICYANIDE 532
One liter sat. sol. in 0.4687 n KOH|contains'342.7 gms. K3Fe(CN)6 at 25°. (Grube, 1914.)
0.91328 302.3 "
1.949 " 215.1 "
100 cc. anhy. hydrazine dissolve 2 gms. K3Fe(CN)6 at room temp.
(Welsh and Broderson, 1915.)
SOLUBILITY OF POTASSIUM FERROCYANIDE IN Aq. POTASSIUM HYDROXIDE
SOLUTIONS AT 25°. (Grube, 1914.)
Gms.
s , K4Fe(CN)6.3H2O
bolvent. per 1000 cc.
Sat. Sol.
308.5 K4Fe(CN)«.3H2O O.Q4I5WKOH 184.8 K,Fe(CN)e.3H20
283.5 " 1-395 " 132-1
247.1 1.883 86.12
217.4
Solvent
0. 09984 W
0.2496
0.4963
0.7036
Gms.
K4Fe(CN)6.3H20
per 1000 cc.
Sat. Sol.
Solid
Phase.
Solid
Phase.
SOLUBILITY OF MIXTURES OF POTASSIUM FERROCYANIDE AND FERRICYANIDE
IN WATER AND IN AQ. POTASSIUM HYDROXIDE SOLUTIONS AT 25°. (Grube, 1914.)
OU1VCLII.
K3Fe(CN)6.
K4Fe(CN)6.
ouiiu jriia.se.
Water
338.1
79.02
K3Fe(CN)6+K4Fe(CN)6.3H2O
0.4687 wKOH
309
66.64
"
0.9628
275-3
55-19
« «
1.949
200.8
35-95
« «
SOLUBILITY OF POTASSIUM FERROCYANIDE IN AQUEOUS SOLUTIONS OF
SODIUM FERROCYANIDE AT 25° AND VICE VERSA. (Harkins and Pearce, 1916.)
Mols. per 1000 Gms. H2O.
Gms.
K4Fe(CN)6 <*2A of
Mols. per 1000 Gms. H2O.
Gms.
Na4Fe(CN)6 <*«.<*
Na4Fe(CN)6.
K4Fe(CN)6". Per 1000 Gms. Sat. Sol.
H2O.
K4Fe(CN)6.
Na4Fe(CN)6.
per i ooo Gms. Sat. Sol.
H2O.
0
O.
89459
329
•5
.09081
0
0.6818
205.
25
1.0595
0.
05072
0.
88272
325
. i
.0990
0.1327
0.7056
2I4.
47
1.0199
O.
06633
0.
88544
326
.10039
o. 1789
0.7213
219.
23
1.0792
0.
12306
0.
88088
324
•4
•09350
0.2115
0.7253
220.
44
i. 1006
0.
25972
0.
89116
328
•3
.12796
o. 2722
0.7610
231.
29
1.1113
0.
4900
O.
91600
337
•4
.17241
0.3532
0.7814
237.
49
1.1243
0.
87034
0.
99000
364
.6
.19700
0.5850
0.8652
262.
97
1.1567
O.
91060
I.
01200
372
• 3
. 21190
o.6m
0.8712
264.
79
1.1581
0.
95879
I.
05177
387
•5
.22673
0.6994
0.8984
273-
05
1.1830
I.
0438
I.
H59
411
•25789
1.0578
0.9588
291.
40
1.2267
POTASSIUM ZINC CYANIDE K2Zn(CN)4.
100 cc. H2O dissolve n gms. K2Zn(CN)4 at 20°. (Sharwood, 1903.)
POTASSIUM FLUORIDE KF.2H2O.
loo gms. H2O dissolve 92.3 gms. KF, or 100 gms. sat. solution contain 48 gms.
KF at 18°. Sp. Gr. of solution = 1.502. (Mylius and Funk, 1897.)
SOLUBILITY OF POTASSIUM FLUORIDE IN HYDROFLUORIC ACID AT 21°.
Gms. per TOO Gms. EfeO.
(Ditte, 1896.)
Gms. per 100 Gms. HgQ.
Gms. per TOO Gms. H2Q.
HF.
0.0
I .21
I.6l
3-73
4-03
6-05
KF.
96-3
72.0
61 .o
40.4
32-5
30-4
' HF.
KF.'
HF.
KF.'
9-25
29.9
20-68
38-4
11.36
29.6
28.60
46.9
12 .50
30-5
41-98
61.8
13-95
31 .4
53-71
74.8
15.98
33-4
74-20
105.0
I7.69
35 -62
119.20
169-5
533 POTASSIUM FLUORIDE
According to de Forcrand (1911), a saturated solution of KF.2H2O in water at
18° has the composition I mol. KF + 3.90 mols. H20 = 45.3 gms. per 100 gms. sat.
solution. The solution in contact with KF.4.H2O as solid phase, has the compo-
sition i mol. KF + 5.76 mols. H2O = 35.96 gms. KF per 100 gms. sat. solution.
EQUILIBRIUM IN THE SYSTEM POTASSIUM FLUORIDE, ETHYL ALCOHOL AND
WATER AT 2^-26°.
(Frankforter and Frary, 1913.)
The authors determined the binodal curve, the quadruple points and two tie lines.
Gms. per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer.
fKF. C2H5OH. H^O? lEi\ QH6OH. H^
1.23 92.67 6.07* 45.33 0.67 54*
... ... 37-82 1.70 60.49
1.16 83.30 15-54
28.68 4.47 66.85
2.86 65.81 31.33
4-47 57-4 38-13 20.90 11.9 67. af
5-47 53 -°4 41-49
18.55 15-6 65.85
6.93 47-52 45-55
8.84 41.28 49.88 15.7 21.8 62. 5t
9-55 38.66 51.79
13-57 27.27 59.15
10.52 35.91 53.57
ii-43 33-23 54-34
ii 30 59 ii 30 59t
* Quad, points. t Tie line. J Plait point approx.
A method for the determination of alcohol in unknown mixtures, based upon the
above data, is described by the authors.
THE BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, PROPYL ALCOHOL
AND WATER AT 2^-26°.
(Frankforter and Frary, 1913.)
Gms. per 100 Gms. Homogeneous Liquid. Gms. per 100 Gms. Homogeneous Liquid.
KF\ C3H7OH. H20." !Ei\ C3H7OH. H^O?
0.17 96.78 3.05* 8.15 7.49 84.36
0.31 78.91 21.19 10 5-97 84.03
0.62 66.29 33.09 12.21 4.39 83.41
0.81 59.97 39.22 14.18 3.45 82.37
1.29 47.46 51.21 18.75 1-89 79-35
i-77 35-40 62.83 25.83 0.74 73.43
2.50 19.05 78.45 35-38 0.23 64.38
5.32 10.64 84.04 47-62 0.039 52-34*
* Quad, point.
One tie line was determined. In this case the upper layer contained 78.91%
C3H7OH and 0.31% KF, and the lower layer contained 9.67% KF.
In this system, the effect of change in temperature is more marked than in
the preceding one in which ethyl alcohol is present.
100 gms. sat. solution of potassium fluoride in 99.6% propyl alcohol contain
0.34 gm. KF at room temp. (Frankforter and Frary, 1913.)
BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, ISOPROPYL ALCOHOL
AND WATER AT 20°.
(Frankforter and Temple, 1915.)
Results in terms of gms. per 100 gms. of solvent, alcohol + water.
Gms. per 100 Gms. Solvent. Gms. per 100 Gms. Solvent.
'KF. CH3CHOHCH3. H2O. 'KK CH3CHOHCH3. H2O/
51.826 1.555 98.445 12.385 21.438 78-562
38.748 2.965 97-035 5-07I 59-339 40.661
36.039 6.525 93-475 3-973 65.455 34-545
17.813 13.215 87.785 1.705 82.750 17-250
POTASSIUM FLUORIDE 534
BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, ALLYL ALCOHOL
AND WATER AT 20°.
(Frankforter and Temple, 1915.)
The results are given in terms of grams per 100 gms. Alcohol + Water instead
of gms. per 100 gms. of the homogeneous mixture.
Gms. per 100 Gms. Solvent. Gms. per 100 Gms. Solvent.
KF. CH2:CH.CH2OH. H2O. KF. CH2:CHCH2OH. H2O.
45.707 2.270 97-730 7.508 35-390 64.610
38.076 3-983 96.017 6.624 42.011 57.989
30.675 5.879 94.121 4.813 47-550 52.450
24.341 7.129 92.871 3.631 54-211 45-789
20.580 9.691 90-309 2.236 59-948 36.443
17.371 11.491 88.509 1.931 65.630 34.370
13.184 17.764 82.236 1-635 68.845 31.155
10.880 22.537 77-463 1.368 71-395 28.605
8.873 29.529 70.471 1-066 75-377 24.223
BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, ACETONE, WATER
AT 20°.
(Frankforter and Cohen, 1914.)
Gms. per 100 Gms. Homogeneous Mixture. Gms. per 100 Gms. Homogeneous Mixture.
r KF. (CH3)2CO. H2O. ^ KF. (CH3)2CO. H2O.
46.3 trace 53.7* 9.17 23.53 67.30
44.24 0.24 55.52 5 38.72 56.28
33.34 i 65.66 3.06 47.89 46.84
29.86 i. 60 68.54 1.38 58.06 40.55
25.74 3.02 71.24 0.979 62.60 36.42
20.28 5.90 73 .80 0.75 65.41 33.84
16.31 9.72 73.97 0.50 69.58 29.92
12.40 15.59 72.01 O 98 2*
* Quad, point.
Data for 4 tie lines are also given and the approximate position of the plait
point is shown on the diagram.
Several points on the binodal curves at temperatures between o° and 35° are
also given.
A discussion, with examples, is given of the applicability of the above data to
the determination of acetone in unknown mixtures.
BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, METHYL ETHYL
KETONE AND WATER AT 20°.
(Frankforter and Cohen, 1916.)
Gms. per 100 Gms. Homogeneous Mixture. Gms. per too Gms. Homogeneous Mixture.
/ A > t A N
KF. CHj.CO.C2Hj. H2O. KF. CHS.CO.C2HB. H2O.
34.38 0.17 65.45 10.50 4.87 84.63
23-63 0.50 75.87 5.70 9.93 84.37
18.62 1.49 79.89 3.96 12.42 83.61
15.91 2.19 81.90 0.84 21.23 77.93
13.80 2.98 83.22 0.34 23.55 76.11
Freezing-point data (solubilities, see footnote, p. i) for mixtures of KF + KI
are given by Ruff and Plato (1903). Results for KF + KOH by Scarpa (1915).
Results for KF + KPO3, KF + K4P2O7 and KF + K3PO4 are given by Amadori
(1912). Results for KF + K2SO4 are given by Karandeef (1909). Results for
KF + NaF are given by Kurnakow and Zemcznzny (1907).
535
POTASSIUM FORMATE
POTASSIUM FORMATE HCOOH.
SOLUBILITY OF POTASSIUM FORMATE AND OF THE ACID SALT IN WATER.
Solid Phase : HCOOK.
A
(Groschuff, 1903.)
Solid Phase : HCOOK.HCOOH.
Cms.
Mols.
Cms. HCOOK.-
Cms.
Cms.
Mob.
HCOOK
HCOOK
HCOOH
HCOOK
HCOOK
HCOOH
t°.
per too
per 100
r.
per 100
per 100
r.
per 100
per i
Cms.
Mols.
Cms.
Cms.
Cms.
Mol.
Solution.
HjO.
Solution.
Solution.
Solution.
HCOOK.
— 2O
72.8
57-4
o
6o-4
39-o
0
36.3
3-21
+ 18
76.8
71.0
25
69.8
4S-i
19-5
38.2
2.96
So
80.7
89.8
50
79-2
51.2
39-3
40.8
2.65
90
86.8
141.0
80
90.7
58.6
60
44.0
2-33
120
92.0
247.0
70
45-9
2.16
140
96.0
5ii
90
S2-!
1.68
157
IOO.O
00
Sp. Gr. of sat. solution at 18° = 1.573.
NOTE. — Since the acid salt is less soluble at ordinary temperatures than the
neutral salt, it can be precipitated from the solution of the neutral salt by addi-
tion of aqueous formic acid. Proceeding in this way an impure product is ob-
tained, giving solubility values (expressed in HCOOK) as shown in the last three
columns above.
POTASSIUM GERMANIUM FLUORIDE K,GeF6.
SOLUBILITY IN WATER.
(Winkler, 1887; Kruss and Nilson, 1887.)
100 gms. H2O dissolve 173.98 gms. K2GeF6 at 18°, and 34.07 gms. at 100° (W.).
100 gms. H2O dissolve 184.61 gms. K2GeF6 at 18°, and 38.76 gms. at 100°
(K. and N.).
POTASSIUM HYDROXIDE KOH.
Gms. KOH per
4°. 100 Gms.
Water.
Solution.
2.2
3-
7
3
.6
20-7
22.
5
18
•4
65.2
44.
5
30
.8
36.2
36.
2
26
.6
32.7
77-
94
43
.8
33
80
44
•4
23-2
85
45
•9
0
97
49
.2
10
103
50
•7
SOLUBILITY IN WATER.
(Pickering, 1893; at 15°, Ferchland, 1902.)
Solid Phase.
Ice
KOH.4H20
KOH.4HjO+KOH.2H2O
KOH.2H,0
Gms. KOH per
t°. 100 Gms.
Solid Phase.
Water.
Solution.
15
107
51-7
KOH.2H2O
20
112
52.8
it
30
126
55-76
"
32-5
135
57-44
KOH.2H2O+
50
I4O
58.33
KOH.H,O
100
I78
64.03
KOH.HjO
125
213
68.06
"
143
3II.7
75-73
ii
Sp. Gr. of sat. solution at 15° = 1.5355.
100 gms. sat. solution in H2O contain 50.48 gms. KOH at 15°.
(de Forcrand, 1909.)
ioo gms. sat. solution in H2O contain 53.1 gms. KOH at 15°.
(Greenish and Smith, 1901.)
POTASSIUM HYDROXIDE 536
SOLUBILITY OF POTASSIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF ETHYL
ALCOHOL AT 30°. (deWaal, 1910.)
Cms. per ioo Cms. Sat. Sol. Gms. per 100 Cms. Sat. Sol.
KOH. QHsOH.
H20.
ooiiu .rnase.
KOH. C2H4OH.
H20.
soiia rb&se.
55
75
0
44-25
KOH.2H2O
27.
67
69
92
2.41
KOH.2H2O
54
,8l
0.43
44.76
"
27.
20
73-
01
negative*
«
Two liquid layers are formed here.
26.
25
81.
95
«
«
31
57.50
11.50
KOH.2H2O
28.
99
65.07
5-94
»
* Negative on account of reaction KOH+QjHjOH— ^QHjOK+HjjO.
Data for equilibrium in the system potassium hydroxide, phenol, water at 25°
are given by van Meurs (1916).
Freezing-point data for KOH + RbOH and KOH + NaOH are given by
von Hevesy (1900). Results for KOH + KI are given by Scarpa (1915).
POTASSIUM IODATE KIO3.
SOLUBILITY IN WATER.
(Kremers, i8s6a; at 30°, Meerburg, 1904.)
t°. 0° 20° 30° 40° 60° 80° 100°
Gms. KI03 per ioo gms. H2O 4.73 8.13 11.73 I2-8 l8-5 24.8 32.2
100 gms. H2O dissolve 1.3 gms. potassium hydrogen iodate, KH(IO3)2, at 15°*
and 5.4 gms. at 17°. (Semllas.)
ioo gms. H2O dissolve 4 gms. potassium dihydrogen iodate, KH2(IO3)3, at 15°.
(Meineke, 1891.)
EQUILIBRIUM IN THE SYSTEM POTASSIUM IODATE, IODIC ACID, WATER AT 30°.
(Meerburg, 1905.)
Gms. per ioo Gms. Gms. per ioo Gms.
Sat. Sol. Solid Phase. Sat. Sol. Solid Phase.
HI03. KI03. " ' HI03. KIOT
O 9.51 KI03 3-47 3-59 KIO3.2HI03 (unstable)
0.65 9.49 « +KI03.HIO, 4-80 2.90
0.65 8.90 KIOj.HIO, 6.45 1.35
0.67 6.6 " 9.35 0.64 KIO3.2HIO3
1.14 4-57 " 12.04 0.44
1.69 3.63 « 17-50 0-30
2. 02 3-10 " 31.20 0.52 "
3.34 2.10 " 53-64 0.68
5 1.32 " 62.52 0.72
7.09 I '« 76.40 0.8o +HI03
8.04 0.85 « +KI03.2HIO3 76.7 O HI03
ioo cc. anhydrous Hydrazine dissolve I gm. KIO3 at room temp.
(Welsh and Broderson, 1915.)
POTASSIUM PerlODATE KIO4.
ioo gms. H2O dissolve 0.66 gm. KIO4 at 13°, dig. of sat. solution = 1.0051.
(Barker, 1908.)
POTASSIUM IODIDE
SOLUBILITY IN WATER, DETERMINED BY THE FREEZING-POINT METHOD.
(Kremann and Kershbaum, 1907.)
Gms. KI per CrtV A Gms. KI per <- KJ
&.<& %£• '"• &.<§£ $2-
-12.5 38 Ice -22.5 52.1 KI
— 15 41.2 " —20 52.6
-17-5 44-6 " -15 53-5
— 20 48 " —10 54-5 "
-22.5 51.2 « - 5 55.4
— 23.2Eutec. 51.9 " +KI o 56.4 "
537
POTASSIUM IODIDE
POTASSIUM IODIDE KI.
SOLUBILITY IN WATER.
(Mulder; de Coppet, 1883; Etard, 1894; Meusser, 1905; see also Tilden and Shenstone, 1884;
Scbreinemakers, 1892.)
Gms. KI per TOO Gms.
Water.
Solution.
10
II5.I
53-5
5
II9.8
54-5
i
122.2
55 '®
0
127.5
56.0
10
136
57-6
20
144
59-O
25
148
59-7
30
152
60.3
40
160
61.5
50
168
62.7
60
176
63-7
70
184
64.8
Gms. KI per 100 Gms.
* .
Water.
Solution.
80
192
65.8
90
200
66.7
100
208
6? 5
no
215
68,3
120
223
69.0
Ice Curve
- 5
25-7
22 5
- 7
42 .6
29.9
- 9
5 5J'5
34-o
— ii
•5 64.7
39-3
-14
75-8
42.7
Sp. Gr. of sat. solution at 15.2° = 1.704. (Greenish and Smith, 1901.)
Individual determinations, in good agreement with the above results, are given
by van Dam and Donk (1911), and by Greenish and Smith (1901).
SOLUBILITY OF POTASSIUM IODIDE + IODINE IN WATER AT 25°.
(Foote and Chalker, 1908.)
Gms. per
100 Gms.
Sat. Sol.
Present in
Solid Phase.
' KI.
I.
I-KI.
29-45
64.34
34.89
Kland
28.91
63.88
34-97
KI3
26.84
27.18
66.54
67.14
39.70
39.96
KI3 and
KI.
27.14
66.00
39.46
Bhlf
Gms. per
100 Gms. Sat. Sol.
Present in
Solid Phase.
' KI.
I. I — KI.
25-88
68.79 42.91
KI7 and
25.57
69.01 43.44
Iodine
27.86
66.56
27.27
66.91
3
26.95
67.17
KI,
25.71
67.91
JXJ.7
The experiments of Hamberger (1906) are discussed. (See also p. 326.)
SOLUBILITY OF MIXTURES OF POTASSIUM IODIDE AND SILVER IODIDE IN
WATER AT o°, 30° AND 50°.
(Van Dam and Donk, 1911.)
Results at o°.
Gms. per TOO Gms. Sat. Sol.
Results at 30°.
Gms. per 100 Gms. Sat. Sol.
Results at 50°.
Agl.
KI.
O
56.1
9
53
18
51-2
3i.3
46.6
37-9
44
37-6
42.7
38
41-3
28.1
36.4
26.6
34-6
6.5
26.1
i-5
20.5
0.2
9.8
27-5
48.7
21
50.3
Agl.
KI.
O
60.35
16
55-5
35-8
46.9
42.8
43-9
44.1
43-2
47-7
40.9
49-7
38.6
42.8
38.8
29.4
37-6
10
31-4
O.I
IO.2
jms. per 100 Gms. Sat. So
I- Solid Phase in
Each Case.
Agl.
KI.
0
62.6
KI
10.7
59-1
«
22.8
55-5
"
45
43-2
tt
53-4
37-6
" +AgI.KI
53-5
37-1
AgLKI
53-5
36-6
" +AgI
53-5
36.5
Agl
39
38.1
28
36.7
«
16
33-8
«
2-5
24.8
"
Agl.aKI+KI
Agl.aKI
POTASSIUM IODIDE
538
SOLUBILITY OF POTASSIUM IODIDE IN DILUTE AQUEOUS SOLUTIONS OF ETHYL
ALCOHOL AT 25°.
(Armstrong, Eyre, Hussey, and Paddison, 1907.)
Wt. Per cent
d of
Gms. KI
Wt. Per cent
d of
Gms. KI
CjHjOH in
Solvent.
SatTSoL
per ioo Gms.
Sat. Sol.
QHsOH in
Solvent.
"25. ^*L
Sat. Sol.
per ioo Gms.
Sat. Sol.
O
1.7268
59.80
4.41
1.6833
58.08
1. 14
I.7I54
59-41
12.14
I . 6063
54-93
2.25
I . 7042
58-95
18.73
1.5420
52.08
loo gms. aqueous 94% ethyl alcohol dissolve 3.99 gms. KI at 17°. (de Bruyn, 1892.)
I oogms. aqueous 98% methyl alcohol dissolve 17.1 gms. KI at 17°.
ioo cc. of ethyl alcohol of di6 = 0.8292 dissolve 8.83 gms. KI at 15°, dm of sat.
solution = 0.8989. (Greenish and Smith, 1901.)
SOLUBILITY OF POTASSIUM IODIDE IN ABSOLUTE ALCOHOLS.
(de Bruyn — Z. physik. Ch. 10, 783, '92; Rohland — Z. anorg. Ch. 18, 327, '98.)
ioo gms. methyl alcohol dissolve 16.5 gms. KI at 20.5°.
100 gms. ethyl alcohol dissolve 1.75 gms. KI at 20.5°.
ioo gms. propyl alcohol dissolve 0.46 gm. KI at i5°-2o° (R.).
SOLUBILITY OF POTASSIUM IODIDE IN:
Ethyl Alcohol
of 0.9496 Sp. Gr.
Aqueous Ethyl Alcohol at 18°.
r
Gms. KI per
Sp. Gr.
Weight
Gms. KI
Sp. Gr.
Weight
Gms. K!
t°.
IOO
Gms. Alcohol
of
Alcohol.
per cent
Alcohol.
per ioo Gms.
Alcohol.
of
Alcohol.
per cent
Alcohol.
per ioo Gms
Alcohol.
8
67.4
0.9904
S-2
I30.5
0.9390
45
66.4
13
69.2
0.9851
9.8
119.4
0.9088
59
48.2
25
75-1
0.9726
23.0
IOO. I
0.8464
86
II.4
46
84-7
0.9665
29.0
89.9
0.8322
91
6.2
55
87-5
0.9528
38.0
76.9
62 9° ' ^ (Gerardin — Ann. chim. phys. [4] 5, 155, '65.^
SOLUBILITY OF POTASSIUM IODIDE IN AQUEOUS SOLUTIONS OF METHYL ALCOHOL
Solvent.
(Herz and Anders, 1907.)
Sat. Solution. Solvent.
Sat. Solution.
Wt. Per cent j
Gms.
KI
Wt. Per cent
Gms. KI"
*•¥>' CH3OH.
"V
per ioo cc. a^'
CH3OH.
«^6-
per ioo cc.
0.9971
O
1.7213
102.
9
0.
8820
64
I
.185
40.33
0.9791
10.
6
1.634
92.
12
O.
8489
78.1
i
.066
28.05
0.9481
30.
8
1.460
55
0.
8167
93-9
0
.9700
18.76
0.9180
47.
i
1.325
55-
6
0.
7881
IOO
0
.9018
13.28
SOLUBILITY OF POTASSIUM IODIDE IN SEVERAL ALCOHOLS.
Alcohol.
Methyl Alcohol
Ethyl
«
Propyl
Amyl
t°.
Gms. KI per ioo
Gms. Alcohol.
Authority.
ii. 4
13-5
(Timofeiew, 1894.)
12.2
14.6
"
13-5
16
"
25
18.04
(Turner and Bissett,
I9I3-)
13.6
1.63
(Timofeiew, 1894.)
25
2.16
(Turner and Bissett,
I9I3-)
12.2
o.73i
(Timofeiew, 1894.)
25
0-43
(Turner and Bissett,
1913-)
25
0.098
«
ioo cc. sat. solution of KI in ethyl alcohol contain 1.585 gms. KI at 25°.
(Laurie, 1912.)
539
POTASSIUM IODIDE
SOLUBILITY OF POTASSIUM IODIDE IN LIQUID METHYL ALCOHOL AT TEM-
PERATURES UP TO THE CRITICAL POINT.
(Tyrcr, 1910.)
(Determined by the Sealed Tube Method.)
r.
15
5 =
5 =
Bo
ICO
14-50
16.20
18.9
22.5
25
r.
140
160
r. ioo
27.2
29.2
30.6
30-7
29.1
240
245
247
250
cnt, temp. 252.5
27-5
24-8
22.6
21
13-8
7-6
SOLUBILITY OF POTASSIUM IODIDE IN VAPOR OF METHYL ALCOHOL ABOVE
THE CRITICAL POINT.
(Tyrer, 1910*.)
GBS-ODiaohrdprriooGi
Btai
:,: =
300
i
33
7
i cc. Vapor.
O.I
O.2
0-3
0.36
0-4
0.45
Data for the
author gives the crit. temp, as 266° and the corresponding concentration as 8.64
gms. KI per ioo gms. of the sat. solution.
0-3
i
3-7*
7-6
ii. 8
18.1
i
3-5
7-4
ti-5
?y~:e~
I
34
73
tt-3
given by
I
3-4
7-2
ii
rszwer (1910). This
SOLUBILITY OF POTASSIUM IODIDE IN MIXTURES OF ALCOHOLS AT 25°.
fliu •ir^a. 1908.)
In Methyl -f Ethyl 1
In Ethyl + Prop>*l
SfiS*1
sSsoL
9SfSSi
•as*
S^SoL ^loT- CSSL~ S.L.SOL ]
per ioo a
Sat-SoL
0
0.8015
i-55
0
O.QOlS
13.16
0
0.8015
1-55
4 37
0.8041
1.91
n. ii
0.8823
IO.O6
8.1
0.7983
1.46
10.4
0.8071
2.25
238
0.8629
8-54
17 85
0.7991
1-37
41.02
0.8295
4 94
65.2
0.8187
2.62
56.6
0.7988
0-75
80.69
0.8794
10.13
91.8
0.8045
0.60
88.6
0.8022
0-52
- --
0.8795
10.72
96.6
0.8041
0.58
91.2
0.8027
0-49
91.25
0.8oo8
11.84
IOO
0.8041
0-43
95 2
0.8029
0-44
ICO
O.OOlS
13.16
IOO
0.8041
0-43
SOLUBILITY OF POTASSIUM IODIDE IN ACETAMIDE.
t» GMS. KI per ioo
Sofid
* -
OK.Sit.SoL
}-_>i
82 m. pt.
O
CHjGOXH-
78
6-5
-
74
12.8
m
70
17-8
"
66
21-5
M
$
26.2
M
53 Eutec,
28.4
•+n
7~
85
ioo
130
145
IOO
175
Gms. KI per ioo
G-B.Sat.5oL
28-75
29.1
29 45
30-15
30-5
30-8
POTASSIUM IODIDE
540
SOLUBILITY OF POTASSIUM IODIDE IN ACETONE AND IN PYRIDINE.
(von Laszcynski, 1894; at 25°, Krug and McElroy, 1892.)
Cms. KI per 100 Cms. Solvent at:
Solvent.
Acetone
Pyridine
— 2.5° 10°
22°
2-38
25°
2-93
56°
I. 21
119°
0.26
O.II
100 gms. glycerol dissolve 40 gms. KI at 15.5°. (Ossendowski, 1907.)
100 gms. 95% formic acid dissolve 38.2 gms. KI at 18.5°. (Aschan, 1913.)
100 cc. anhydrous hydrazine dissolve 175 gms. KI at room temp.
(Welsh and Broderson, 1915.)
100 gms. hydroxylamine dissolve no gms. KI at 17.5°. (de Bruyn, 1892.)
100 gms. sat. solution in hydrated lanolin (containing 30% emulsified water)
contain 42.5 gms. KI at 45°. (Klose, 1907;) KI is insoluble in anhydrous
lanolin.
SOLUBILITY OF POTASSIUM IODIDE IN SEVERAL SOLVENTS.
(Walden, 1906.)
Solvent.
Water
Water
Methyl Alcohol
Methyl Alcohol
Ethyl Alcohol
Ethyl Alcohol
Glycol
Glycol
Acetonitrile
Acetonitrile
Propionitrile
Propionitrile
Benzonitrile
Nitromethane
Nitromethane
Nitrobenzene
Acetone
Acetone
Furfurol
Furfurol
Benzaldehyde
Salicylic Aldehyde
Salicylic Aldehyde
Anisic Aldehyde
Anisic Aldehyde
Ethyl Acetate
Methyl Cyanacetate
Methyl Cyanacetate
Ethyl Cyanacetate
_ .
*« SD.Gr.of oms.^perioo
1* orrnula,.
Solution.
cc. Solution. Gms. Solution.
H2O
o i . 6699
94-05
56.32
H2O
25 I-7254
IO2 . 70
59-54
CH3OH
o 0.8964
ii. 61
12.95
CH3OH
25 0.9003
13.5-14.3
14.97
C2H5OH
o 0.8085
1.197
1.479
C2H5OH
25 0.7908
1.520
1.922
(CH2OH)2
0 1-3954
45-85
31-03
(CH2OH)2
25 1.3888
47-23
33-01
CHgCN
o 0.8198
1.852
2.259
CH3CN
24 0.7938
i-57
2.003
C2H5CN
o 0.8005
0.34-0.41
0.0429
C2H5CN
25 0.7821
0.32-0.36
0.0404
C6H5CN
25
[.0076
0.051
0.0506
CH3NO2
0
[.1627
0.314-0.366
0.315
CH3NO2
25 1.1367
0.289-0.349
0.307
CeHsNC^
25
. . .
0.0019
(CH3)2CO
o 0.8227
1.732
2.105
(CH3)2CO
25 0.7968
1.038
1.302
CAO.COH
0
15. 10
. . .
C4H3O.COH
25
.2014
5.62
4-94
C6H5COH
25
.0446
0.343
0.328
C6H4.OH.COH
o
• 1501
1.257
1.093
C6H4.OH.COH
25
•1373
0.549
0.483
C6H4.OCH3.COH
o
.1223
1.520
1-355
CeH4.OCH3.COH
25
.1180
0.720
0.644
CH3COOC2H5
25
. . .
0.0013
CHoCNCOOCHg
o
.1521
3.256
2.827
CH2CNCOOCH3
25
.1358
2.459
2.165
CH2CNCOOC2H5
25
.0628
0.989
0.930
541 POTASSIUM IODIDE
SOLUBILITY OF POTASSIUM IODIDE AT 20° IN SEVERAL SOLVENTS CONTAINING
DISSOLVED IODINE.
(Olivari, 1908.)
Gm. Mols. KI per Liter in Solvent Containing:
Solvent. as Gm. Mols. Ts~Gm. Mols. 2.5 Gm. Mols.
I2 per Liter. Ij per Liter. I2 per Liter.
Acetic Acid 0.511 1.460 2.080
Ethyl Acetate 0.490 1.400 1.980
Ethyl Alcohol 0.520 1.220 1.730
Nitrobenzene 0.414 0.960 1.380
Ethylbromide 0.140 0.350
EQUILIBRIUM IN THE SYSTEM POTASSIUM IODIDE — ETHYL ETHER — WATER AT 20°.
(Dunningham, 1914-)
Cms. per too Gms. Upper Layer. Gms. per 100 Gms. Lower Layer. Solid
KL~~ ~~HA (C2H6)20. liL*"" H2O. (QH^O. Phase-
59-2 40.8 ... KI
o 3.9 96.1 o 93 7 None
0.4 0.4 99-2 55-6 40-7 3-7 KI
O.I 2.2 97.7 25 72.1 2.9 None
DISTRIBUTION OF POTASSIUM IODIDE BETWEEN WATER AND:
Nitrobenzene at 1 8°. (Dawson, 1908.) Phenol at Room Temp. (Riesenfeld, 1902.)
Mols. KI per Liter. Dist. Gms. KI per 100 cc. Dist.
CeHfiNOz Layer"! H2O Layer. Ratio. C6H6OH Layer! Aq. Layer.' Ratio.
O.OOII4 6.05 5300 0.052 0.725 13.2
0.00108 6.05 5600 0.197 2.42 12.3
2.09 30.7 14-7
Freezing-point data for KI + K2SO4 and KI + NaCl are given by Ruff and
Plato (1903). Results for KI + Agl are given by Sandonnini (i9i2a). Results
for KI -f- SO2 are given by Walden and Centnerszwer (1903).
POTASSIUM IODOMERCURATE (Thoulet Solution).
A sat. solution at 22.9°, prepared by adding KI and HgI2 in excess to water,
contained 8.66% K, 22.49% Hg, 52.58 (57.7) % I and 10.97 (11.15)% H2O,
corresponding to 0.22 mol. alkali, o.n mol. Hg and 0.45 mol. I. (Duboin, 1905.)
POTASSIUM MOLYBDATE K2MoO4
SOLUBILITY OF POTASSIUM MOLYBDATE IN AQUEOUS SOLUTIONS OF POTASSIUM
SULFATE AT 25° AND VlCE VERSA.
(Amadori, igi2a).
Gms. per 100 Gms. H2O. Gms. per 100 Gms. H2O.
fzSOT K2MoO4: KjSOT K2MoO4.'
o 184.6 1.50 99-49
0.46 180.7 2-T3 45-89
0.72 177 3.95 17-48
0.98 127.2 8.55 4-73
1.27 JO7.5 12. 10 o
Freezing-point data for K2MoO4+ K2SO4, K2MoO4 + K2WO4 and K2Mo2O
+ K2W2O7 are given by Amadori (1913).
POTASSIUM NITRATE KNO3.
SOLUBILITY ICE CURVE AND SUPERSOLUBILITY ICE CURVE.
(Jones, 1908.)
Gms. KNO3 per 100 Gms. H2O. Gms. KNO3 per 100 Gms. H2O.
of Cryst Solubility Supersolubility o{ Cryst. Solubility Supersolubility
Ice Curve. Ice Curve. Ice Curve. Ice Curve.
-I 3.336 I. Oil -3 ... 5.762
— 2 7.582 3-S38 —4 ... 8.694
— 2.8* 11.62 5.56 —5 .... II. 12
-5-3* ... ".82
* Cryohydrate.
POTASSIUM NITRATE 542
SOLUBILITY IN WATER.
(Mulder; Andrae, 1884; Gerardin, 1865; Etard, 1894; Ost, 1878; at 31.25°, Kohler, 1897; Euler, 1904;
Tilden and Shenstone, 1884; Berkeley, 1904.)
Average Curve.
9 Gms. KNOa per TOO Gms. . Gms.KNO3 per TOO Gms.
Water. Solution. Water. Solution.
o 13-3 11.7 70 *38 58 o
10 20.9 17.3 80 169 62.8
2O 3I-6 24.O 9O 2O2 66.9
25 37.3 27.2 ioo 246 71.1
30 45-8 3J-4 no 300 75.0
40 63.9 39.0 120 394 79-8
50 85.5 44-o 125 493 83.1
60 no.o 52.0
The very carefully determined figures of Berkeley are as follows:
dt of
Gms. KNOs per
d.oi
Gms. KNO3 per
Sat. Sol.
ioo Gms. H2O.
'
Sat. Sol.
ioo Gms. HjO.
0.40
1.0817
13-43
60.05
I-3903
111.18
14.90
1.1389
25.78
76
1.4700
156.61
30.8o
I.22I8
47-52
91.65
1-5394
210.20
44-75
i-3°43
74.50
114 b. pt.
1.6269
311.64
IOOO gms. H2O dissolve 384.48 gms. KNO3 at 25°. (Armstrong and Eyre, 1910-11.)
One liter sat. solution in water contains 2.8 mols. = 283.11 gms. KNO3 at 20°.
(Rosenheim and Weinheber, 1910-11.)
Recent determinations of the solubility of potassium nitrate in water, agreeing
satisfactorily with the above data, are given by Chugaev and Khlopin (1914).
SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND BARIUM
NITRATE IN WATER.
(Euler — Z. physik. Ch. 49, 313, '04.)
t°. Sp. Gr. of Sat. Solution. Grams per ioo Grams H2O.
17 1. 120 13.26 KNO3+ 6.31 Ba(NO3)2
21.5 ... 17.00 " + 7-58
30 1.191 24.04 + 9-99
50 ... 49-34 +18.09
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC
ACID AT o°.
(Engel — Compt. rend. 104, 913, '87.)
p. Gr. of
olutions.
Equivalents
per 10 cc. Solution.
Grams per ioo cc. Solution.
1.079
i2.5KN03
o HN03
12.65 KNO3 o.ooHNO8
9-9 "
5-87
H
IO-O2 "
3-71
tt
•093
8.28 "
13-2
tt
8.38 "
8.38
"
.117
7-4 "
2i-55
tt
7-49 "
13.58
"
.144
7-4 "
3i-i
tt
7-49 "
19.47
"
.202
7.6 «
48.0
tt
7.68 "
30.04
"
.289
10.3
68.0
tt
10.42 "
42.86
tt
498
28.3 "
120.5
tt
28.64 "
75-95
"
Freezing-point data for KNO, + HNO3 are given by Dernby (1918).
543
POTASSIUM NITRATE
SOLUBILITY OF POTASSIUM NITRATE AND OF ACID POTASSIUM NITRATES
IN NITRIC ACID.
(Groschuff — Ber. 37, 1490, '04.)
NOTE. — Determinations made by the so-called thermometric
method, i.e., by observing the temperature of the disappearance of
the separated, finely divided solid from solutions of known concen-
tration.
Grams per 100
t°. Solution.
Gms.
Solid
Phase.
Gms. per 100 Gms.
t °i Solution.
Solid
Phase.
KN03.
HNO3.
K.N03. HN03.
- 6
24
•4
75
.41
KNO3.2HNOa 0)
22.5
47.2
52-93
KN03.HN03
+ 14
32
.6
67
.42
" (stabil)
23-5
47.8
52.11
" (stabil)
17
34
.8
65
.04
"
25-5
48.6
51.46
«'
19
•5 37
.2
62
.90
"
27.0
49.4
50.78
22
44
•5
55
.46
"
29.0
50.1
49.94
KNO3.HNO3
21
•5 47
.8
S2
.11
KNOs.2HNO3 (0
30-5
5o-9
49-15
(labil)
21
•5 48
.6
51
.46
(labil)
21 .0
49.4
50.78
KNO8 (labil)
20
So
•9
49
.15
"
39-o
5o-9
49 -IS
" (stabil)
— 4
37
.a
62
-8l
KNO3.HNO3
5°
51 .7
48.32
-16
•5 44
•5
55
.46
(labil)
c1)
Solution in HNO3.
0)
Solution in
KNOj.
CONDUCT
OF
ACID POTASSIUM
NITRATE TOWARDS
WATER.
Gms. per 100 Gms.
t°. Solution.
Solid
Phase.
t°
Gms. per 100 Gms.
Solution.
Solid
Phase.
KN03.
HN03.
KNOg.
HNO3.
22
44
•5
55
•5
KNO3.2HNOi
5°
38.
7
48.
3
KNO8
20
•5 44
.1
55
• o
"
61
36.
o
44-
8
"
18
43
.8
54
•5
"
63
34-
5
43-
o
"
12
43
• 0
53
.6
"
60.
5 3°-
39-
5
"
6
42
•3
52
•7
"
56
27.
6
34-
4
"
o
41
.6
51
.8
"
43
20.
8
25-
9
"
12
41
•3
51
•4
KNO8
17
ii. 7
14.
6
M
22
40
•9
51
.0
it
-5
5-
54 6.91
40
39
•9
49
.8
*
SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND POTASSIUM
CHLORIDE IN WATER.
(Etord — Ann. chim. phys. [7] 3, 283, '94; at 20°, Riidorff — Ber. 6, 482, '73; Nicol — Phil. Mag. [5]
3 it 385, '91 •)
Gms. per too Gms.
t». Solution.
Gms. per 100 Gms.
40. Solution.
Gms.
t°.
per 100 Gms.
Solution.
KN03.
KCI/
'KN03.
KCI:
KN03.
KCI.
0
5-o
20. o
30
16
• o
21
.2
70
39
•5
17-5
10
8.0
20.8
40
21
.0
21
• O
80
45
^5
15-8
20
12.6
21 .2
50
27
• o
2O
• O
100
57
•5
ii .6
25
14.0
21.3
60
33
•5
19
.0
120
69
• 0
7-7
POTASSIUM NITRATE
544
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OP:
(Touren — Compt. rend. 131, 259, 'oo.)
Potassium Carbonate.
Results at 14.5°.
Potassium Bi Carbonate.
Mols. per Liter.
Gms. per Liter.
KzCO*.
KNOa-
K2C03.
KJNU3.
o.o
2
.228
o.o
225
0-48
I
•85
66.4
188
1-25
I
•39
172.9
141
2.58
0
.86
356-9
87
3-94
o
.64
544-9
65
Results at
*s°.
o.o
3
.217
o.o
326
o-59
2
.62
81.6
265
3-35
I
•97
186.7
199
2.10
I
.46
290.5
148
2.70
I
.14
373-6
H5
3-58
O
•79
495 -1
80
Results at
Mols. per Liter.
14-5°.
Grams per Liter.
KHC03.
KN03. KHC03.
KN03.
0-0
2-33
o.o
336
o-39
2.17
39-o
2 2O
0.76
2.03
76.0
205
1.16
1.92
116
194
i-55
1.81
J55
183
Results at
25°.
o.o
3-28
o.o
332
0.89
2.84
89
287
i-33
2.65
133
268
1.91
2-45
191
249
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CARBONATE AT 24.2°.
(Kremann and Zitek, 1909.)
Gms. per 1000 Gms. H2O.
KNO3.
Gms. per 1000 Gms. H2O.
KN03.
376.8
285
161.7
I4I.8
K2C03.
O
I30-3
348.4
371-9
Solid
Phase.
KNO,
73
38.8
K2C03.
688.1
878.3
III2.2
Solid
Phase.
KNO3
+K2CO,
looo gms. H2O containing I mol. KC1 (ioi.n gms.) dissolve 324.85 gms. KNO3
at 25 . (Armstrong and Eyre, 1910-11.)
Data for the system potassium nitrate, potassium sulfate, water at 35° are
given by Massink (1916, 1917).
SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND POTASSIUM
SULPHATE IN WATER.
(Euler — Z. physik. Ch. 49, 3i3> '04-)
t*. Sp. Gr. of Sat. Solution. Grams per 100 Grams Water.
15 i . 165 24 .12 KNO3 " 5.65 K2SO4
20 ... 30.10 " 5.58 "
25 I. 210 36.12 " 5.58 "
SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND SODIUM
CHLORIDE IN WATER.
(Etard — Ann. chim. phys. [7] 3, 283, '94
agree well with those of Etard.)
; the older determinations of Riidorff, Karsten, Mulder, ;tc.
t».
Gms. per 100 Gms.
Solution.
t°.
Gms. per 100 Gms.
Solution.
t°.
Gms. per 100 Gms.
Solution.
KN03. NaCl. "
KNO3. NaCl."
KNO3. NaCl.
0
13 24
40
3o-5 *9
120
73 8.0
10
16 23
So
36 17
140
77 7-o
20
2O 22
60
42-5 15
160
79-5 6-°
25
23 21-5
80
55 12
170
80.5 5-5
30
25 20.5
100
67 9-5
545
POTASSIUM NITRATE
100 gmsi H2O, simultaneously sat. with potassium nitrate and sodium chlo-
ride, contain 41.14 gms. KNO3 + 38.53 gms. NaCl at 25° and 168.8 gms. KNO8
+ 39.81 gms. NaCl at 80°. (Soch, 1898.)
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AND VICE VERSA. (Leather and Mukerji, 1913.)
Sp. Gr.
Results at 20°.
Gms. per 100 Gms. H2O.
Solid
Sp. Gr.
Results at 30°.
Gms. per looGms. H2O.
Solid
Sat. Sol.
' KNO3.
NaCl.
Phase.
Sat. Sol.
KNO3.
NaCl.
Phase.
1.167
31
•49
0
KNO,
I
.261
46
.48
9.82
KNO,
I.22O
33
.41
9-
94
«
I
• 302
47
.08
20. l8
«
1.267
34
•93
19.
44
"
I
•343
47
.24
29.86
«
I.3II
36
.41
29.
46
ii
I
•372
49
.24
38.72
" +NaCl
1-344
37
•30
37-
73
" +NaCl
I
•342
38
•36
38.55
NaCl
1-330
31
.41
37-
57
NaCl
I
.298
25
•32
38.23
»
1.283
19
•56
37-
"
I
.258
12
•IS
37.38
«
1-243
9
.76
36.
73
"
I
.202
36.30
"
Results at
40°.
Results
at 91°.
1.288
64
•74
o
KNO,
I
-552
2O2
.8
o
KNO,
1.320
64
.66
ii.
32
"
I
•573
204
.2
12. 8l
ii
. . .
64
•05
23-
41
"
.601
208
.1
28.45
«
1.396
64
•13
35-
08
«
•645
213
•3
37-92
»
1.411
64
•77
38.
79
" +NaCl
.660
218
.8
39-oS
" +NaCl
1.376
52
.81
39-
51
NaCl
.607
175
.8
40.87
NaCl
1-323
34
•98
38.
98
"
•517
126
•9
44-33
. ii
1.267
17
•33
37-
74
a
•378
57
•53
42.90
,
At the higher temperatures, results for NaNO3 in certain solutions are reported.
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND VICE VERSA. (Leather and Mukerji, 1913.)
Rei
Sp. Gr.
Sat. Sol.
I.3I7
1.403
1.472
1-544
1.520
1.481
I-451
1.406
suits at 30°.
Gms per 100 Gms.
H20.
Res
Sp. Gr.
Sat. Sol.
1.358
1.428
I-505
1-570
1-573
1.526
1.476
1.421
mlts at 40°.
Gms. per 100 Gms.
H20.
Sp. Gr.
Sat. Sol.
1.615
1.674
I-75I
1.790
1-774
1.695
1.610
1.521
Results at 91
Gms. per 100 Gms.
H2O.
o
Solid Phase
in
Each Case.
KNO,
«
" +NaNO,
NaNO,
«
KN03.
45-73
47-25
50.93
54-34
47.67
30.25
14.30
0
NaN03."
25.90
52.53
79.27
103.3
103.1
101.6
99.10
95-90
KN03.
63.21
63.86
66.44
74.06
68.72
43-92
20.33
0
NaN03.
23.85
49-79
79.46
116.2
116.7
112. 2
109.9
105.2
KN03.
200.8
207.2
229-5
251.8
2II.7
128.5
.55-75
o
NaN03."
43-4 :
92.90
156.2
206.5
200
186
I73.I
160.8
Results at 20° are also given.
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND VICE VERSA AT 20°.
(Carnelly and Thomson — J. Ch. Soc. 53, 782, '88; Nicol — Phil. Mag. 31, 369, '91.)
KNO3 in Aq. NaNO3 Solutions. NaNO3 in Aq. KNO3 Solutions.
Grams per 100 Grams HaO.
KNO3. NaNO3. "
88
90
92
93
Grams per 100 Grams H2O.
NaNO3. KN03
O
10
20
40
60
80
31-6
30-5
3I.O
33-o
35-5
41-0
o
10
20
25
30
35
94
96
POTASSIUM NITEATE
546
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND VICE VERSA AT 10° AND AT 24.2°.
(Kremann and Zitek, 1909.)
Gms. per 1000 Gms. H2O.
Cms. per 1000 Gms. H2O.
I .
KN03.
NaN03.
OUUU JTllitSC.
*
KNO3.
NaN03.
ouiiu ruMBi
10
208.9
O
KNO3
24.2
422
931-3
KNO,
IO
301.9
848.3
" +NaNO,
24.2
437
1019
" +NaNO,
IO
o
805
NaNO,
24.2
123.6
910.6
NaNO,
24.2
377-3
0
KNO,
24.2
o
913
"
24.2
390
346.7
"
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF SILVER NITRATE
Gms. per too Gms. Sat. Sol.
KNO3.
31-3
30-45
29.22
26.58
25.02
AgN03.
o
11.51
23-59
39-09
46.38
AT 30° AND VICE VERSA.
(Schreinemakers, 1908-09.)
Solid Phase.
KNO,
" +AgNOj.KNO3
KNO3.
AgN03.
ounu rna.sc
17.38
57-85
AgNOj.KNO,
13-44
65.08
«
11.22
69.01
" -hAgNO,
5-53
7I.6S
AgNO,
0
73
"
SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND SILVER NITRATE
Gms. per 100 Gms. Sol.
o
10
20
25
KNO3.
13-5
19
23
25
AgNO3.
43
44-7
47
48
IN WATER.
(Etard, 1894.)
Gms. per 100 Gms. Sol.
' KNO3. 'AgNO3.
Gms. per 100 Gms. Sol.
30
40
26.8
29.6
32
33-5
49-4
Si-5
54
54-8
80
IOO
120
140
KNO3.
36-2
38.3
40
41-5
AgNO,.
55-1
55-3
55-6
55-8
SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM NITRATE AND SILVER
Gms. per Liter.
NITRATE IN WATER AT 25°.
(Herz, 1905; Fock, 1897.)
Mg. Mols. per Liter.
Mol. Per cent Mol. Per cent
AgN03.
45-9
110.7
176.8
259.6
365-6
507-9
745-9
KNOj.
321.8
322.6
333-7
364
456.4
387.2
398.6
AgNO3.
270
65L3
1040
1528
2151
2988
4388
KNO»
3180
3184
3298
3597
45"
3816
396o
AgN03 in
AgNO3 in
Solution.
Solid Phase.
7.83
0.2896
16.96
0.6006
23-97
o . 9040
29.81
1-054
32.28
1.604
43-85
2-439
52.70
8.294
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF STRONTIUM
NITRATE AND VICE VERSA AT 20° AND AT 40°.
(Findky, Morgan and Morris, 1914.)
Gms. per 100 Gms.
t°. Sat. Sol. Solid Phase. t°.
Gms. per
Sat.
100 Gms.
Sol.
Solid Phase.
KNOj.
Sr(NOj)2.
' KNOj.
Sr(NO3)2.
20
22
90
5.49 KNO,
20
12
-65
41.
12
Sr(N03)2.4H20
2O
21
70
9.17
2O
10
40.
70
"
2O
21
OI
17.10 '
40
30
.26
23-
70
KNO3
20
19
60
31.24
40
26
.90
38.
52
" +Sr(NOj)2.4H20
2O
19
49
34-91
40
22
•50
40.
22
Sr(NO,)2.4H20
2O
19
69
39.56 ' +Sr(N03),.4H20
40
II
.19
44-
19
"
20
17
56
40.37 Sr(NO3)2.4H2O
40
O
47-
7
"
1000 gms. H2O, simultaneously saturated with both salts, contain 552 gms.
KNOi + 1074 gms, Sr(NO3)2 at 25°, (LeBlanc and Noyes, 1890.)
547
POTASSIUM NITRATE
SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM NITRATE AND THAL-
LIUM NITRATE IN WATER AT
(Fock.)
*$'
Grams per Liter.
Mg.
Mols. per Liter.
Mol. per cent Sp. Gr.
T1NO* of
Mol. per cent
TINOa
T1NO3.
KN03.
T1N03.
KNO3
, in Solution. Solutions, in Solid Phase .
O-OO
351
.0
0
.0
3468
.2
O
.00
.2632
O
.00
2-37
329
.0
8
•9
3251
•5
O
•43
.1903
0
.08
6.15
332
•4
23
.1
3285
.1
0
.70
.1956
0
.20
17.64
333
•7
66
•3
3298
.1
I
•97
.2050
o
•57
49-74
333
•3
186
•9
3294
•4
5
•37
.2196
I
.78
63.60
321
.0
239
.0
3172
•4
7
.01 1.2436
2
.19
86.18
330
•5
323
.8
3265
.8
9
.02 1.2617
2
•77
123.8
428
•3
465
.2
4232
.6
9
.90 1.2950
(27
.00
.04
101.3
245
.1
380.6
2423
•3
13
.58 1.2050
93
•33
116.1
o
.0
463
.1
O
.0
100
.00 i .0964
IOO
.00
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL SOLUTIONS,
(Gerardin — Ann. chim. phys. [4] 5, 151, '65.)
Grams KNO3 per 100 Grams Aqueous Alcohol of Sp. Gr.:
t°.
0.9904
0.9843
0.9793
0.9726
•09571
0-939
0.8967
0.8429
= 13-6
= 19.1
= 40
= 60
=90
Wt.%.
Wt.%.
Wt.%.
Wt.%.
Wt.%.
Wt.%.
Wt.%.
Wt.%.
10
i7
13
10
7
4-5
3
I
0-2
18
22.5
18.5
14-5
10
6.2
4-5
1.6
0-3
20
24
20
16
ii
7.0
5
2
o-3
25
29
24-5
20
13-5
9.0
6-5
2-5
0.4
30
36
30
25
8
0.5
40
52
43
36
27
16:5
ii
4
0.6
5o
72
61
50
38
23.0
16
6
0.7
60
93
79
69
52
31.0
21
8
i.i
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL AT 18°
(Bodlander — Z. physik. Ch. 7. 316, '91.)
p. Gr. of
Gms. per 100 cc. Solution.
Sp. Gr. of
Gms. per 100 cc. Solution.
Solution.
C^OH.
H2O.
KN03.
Solution.
C2H6OH.
H20.
KNOa".
I .1480
.
89
.80
25.0
I
.0120
23-33
69.81
8.06
.1085
3
•3o
87
•44
2O- 1 1
O
•9935
28
.11
64.74
6.50
• IOIO
5
.24
86
.26
18.60
0
•9585
37
•53
54-21
4-II
.0805
8
.69
83
.18
16.18
o
•9450
42
.98
48.15
3-37
•0755
9
.06
83
.10
15 .39
o
.9050
51
•23
27.32
i-95
•0655
14
.08
77
•93
14-54
o
.8722
61
•65
24.74
0.83
.0490
16
.27
76
•36
12.27
o
•8375
69
.60
13-95
O-2O
•0375
19
•97
72
•93
10.8
SOLUBILITY OF POTASSIUM NITRATE IN DILUTE ETHYL ALCOHOL AT 25°.
(Armstrong and Eyre, 1910-11.)
Wt.% '
QHsOH in
Solvent.
O
2.25
4.41
Gms. KNOj
per 100 Gms.
Sat. Solution.
27.77
26.69
25-79
23.81
POTASSIUM NITRATE 548
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL AND IN AQUEOUS
ACETONE.
(Batnrick, 1836.)
In Aqueous Alcohol. In Aqueous Acetone at 40°.
Wt Per cent Gms. KN03 per 100 Gms. Aq. Alcohol. Wt. Per cent Gms. KNO3
Alcohol. ' At30o. At 40°. ^ Aceto- ^XnGtmS-
o 45-6 64.5 o 64.5
8.25 32.3 47-i 8.5 51.3
17 22.4 33.3 16.8 38.9
25.7 15.1 24.1 25.2 22.8
35 11.4(34-4°) 16.7 34.3 24.7
44-9 7 11.6(44°) 44-1 17
54-3 4-5 7-2(55) 53-9 "-9
65 2.7 4-4 64.8 7.2
75-6 1.3 2 (76.3) 76 3
88 0.4 0.6(88.5°) 87.6 0.7
100 gms. H2O saturated with sugar and KNO3 dissolve 224.7 E^s. sugar -f-
41.9 gms. KNO3, or 100 gms. of the saturated solution contain 61.36 gms. sugar
+ 11.45 gms. KNO3 at 31.25°. (Kohler, 1897.)
SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF METHYL
ALCOHOL, ETHYL ALCOHOL AND MIXTURES OF THE Two AT 30°.
(Schreinemakers, 1908-09.)
In Aq. CH3OH. In Aq. C2H5OH. In Aq. v^xi3v^**T^2iX6^
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
CH3OH. KNO3. QHjjOIL KNO3. '(CH3OH +0^011) KNO3.
o 31.3 10. i 20.7 o 31.3
7.8 23.3 23.8 12. 1 12.7 18.9
17.3 16.3 32.2 9 29.2 12.8
27.8 ii. 2 43.1 6.1 41 6.7
38-4 7-7 56.9 3-3 47-8 5-*
57 3-8 76-8 0.88 56.4 3.5
98.58 0.43 92.3 0.15 74.8 1.2
* The mixture contained 51.7% CH3OH and 48.3% C2H5OH.
loo gms. trichlorethylene dissolve o.oi gm. KNO3 at 15°. (Wester and Bruins, 1914.)
100 cc. anhydrous hydrazine dissolve 14 gms. KNO3 at room temp.
(Welsh and Brpderson, 1915.)
100 gms. aq. 40 weight % C2H6OH, simultaneously saturated with the two
salts, dissolve 13.74 Sms- KNO3 + 15.78 gms. NaCl at 25°. (Soch, 1898.)
SIMULTANEOUS SOLUBILITY OF POTASSIUM NITRATE AND SILVER NITRATE IN
AQUEOUS 51.6 PER CENT C2H6OH AT 30°.
(Schreinemakers, 1908-09.)
Gms. per 100 Gms. Sat. Solution.
-KNCV • AiNoT SoMK— '
4-8 o KNO3
4-55 5-15
4.11 16.47
4-26 21.28 " H-AgNO3.KNO,
2.62 36.94 AgN03.KNO3+AgNO,
o 37 AgN02
Fusion-point data (solubilities, see footnote, p. i), are given for KNO3 + KNO2
by Meneghini (1912); for KNO3 + AgNO3 by Usso (1904); for KNO3 + NaNO3
by Carveth (1898) and by Hissink (1900); for KNO3 + Sr(NO3)2 and KNO3
+ NaNO3 + Sr(NO3)2 by Harkins and Clark (1915); for KNO3 + T1NO3 by
Van Eyk (1899, 1905).
549
POTASSIUM NITRITE
POTASSIUM NITRITE KNO2.
SOLUBILITY IN WATER.
(Oswald, 1912, 1914.)
Gms. KNO2 «, ,. .
- 4.1
- 7-6
-13.8
-18.6
— 24.6
-30
— 31.6 Eutec.
16.1
24.1
40.2
50.1
61.7
69.8
71.8
73-2
73-6
Ice
" +KN02
KN02
* dn.i = 1.6464.
• 17-
25
40
55
75
100
in
119
100 gms. H2O dissolve about 300 gms. KNO2 at 15.5°.
The figure 138.5 gms. KNO2 per 100 gms. H2O at 15°,
towski and von Roszkowski (1897), is evidently low.
Cms. KNOj
per 100 Cms.
Sat. Sol.
Solid
Phase.
74-5*
KNOj
75-75
"
77
«
77-5
M
78.5
«
80.5
«
80.7
II
81.15
«
81.8
«
(Divers, 1899.)
given by von Niemen-
SOLUBILITY OF MIXTURES OF POTASSIUM NlTRITE AND OF SILVER NlTRITE IN
WATER.
(Oswald, 1914.)
Results at 13.5°.
Gms. per 100 Gms. H2O.
Results at 25°.
Gms. per 100 Gms. H2O.
kN02.
18
276
AgN02.
2.36
26.3
KN02.
23.1
279
AgN02.
5-3
39-3
Solid Phase in Each Case.
AgN02+K2Ag2(N02)4.H20
KN02+K2Ag2(N02)4.H20
Of the two layers obtained by mixing an equal volume or more of 96% ethyl
alcohol with a nearly saturated aqueous solution of KNO2, the lower contains
71.9% KNO2 and the upper, alcoholic, 6.9%. With methyl alcohol there is no
separation into two layers. (Donath, 1911.)
POTASSIUM OXALATE K2C2O4.4H2O.
SOLUBILITY OF MIXTURES OF POTASSIUM OXALATE AND OXALIC ACID IN
WATER AT 25°.
(Foote and Andrew, 1905.)
Gms. per 100 Gms. Solution.
H2C204.
K,Q04.
IO.2
10.31
0.04
9.26
0.13
3-39
0.63
2.06
4.26
1.16
11.50
0.99
16.93
0.85
21. 08
0.82
21.49
0.64
23-52
0-57
24.88
0-43
27.52
27.40
Mols. per 100
Mols. H2O.
2.274
K2C204.
2.302
2.046
0.005
0.016
0.707
0.071
0.440
0.266
0-495
1.427
0.240
0.221
0.2II
0.169
0-153
2.235
2.928
2.998
3-301
3.617
0.122
4.14
4.09
Solid Phase.
H2C2O4.2H2O+H3K(C2O4)2.2H2O
Double salt H3K(C2O4)2.2H2O
H3K(CA) .2HJO+HKCA
Double salt HKC-A
HK CA +H2K4(C204)3.2H20
Double salt H2K4(C204)8.2H2O
HSK4(CS04)3 2H2O4-K,C5O4.H2O
POTASSIUM OXALATES
550
EQUILIBRIUM IN THE SYSTEM POTASSIUM OXALATE, OXALIC ACID, WATER AT
o°, 30° AND 60°.
(Koppel and Cahn, 1908.)
Results at o°.
Gms. per 100 Gms.
Sat. Sol.
Results at 30°.
Gms. per 100 Gms.
Sat. Sol.
Results at 60°.
Gms. per 100 Gms.
Sat. Sol. Solid Phase in Each Case
CA.
2.72
2.91
K20.
O.226*
Q03.
9-97
10.15
K20.
O.IO
C203.
24-75
K20.
2.
985
0
•342*
. .
2.
827
o
.125
IO.
23
0.
34
25
.70
O.
46 " +KH3(C2O4)2.2H2O
2.
345
o
•145
. .
.
. .
.
.
" "
I.
47i
o
195
7-
28
o.
33
25
.So
O.
54 KH3(QO4)2.2H2O
0.823
o
.240
4
0.
4i
22
.06
o.
58 "
O.
799
o
454
3-
08
0.
50
20
• 17
0.
67 "
I.
173
o,
.785
2.
38
I.
002
14
• 25
o.
90
I.
38i
0
962
2.
98
I.
79
9
.82
I.
48 "
I.
545
I,
155
. .
6
•95
2.
244 "
I.
666
I,
273
4-
24
2.
76
9
•17
5-
60 " +KHCA
I.
754
I.
479
4-
26
3-
38
8
.81
6.
37 KHCA
2.
627
2,
858
5-
44
5-
43
10
•17
10
"
3-
772
4.
422
6.
66
7-
27
12
•36
13.
40
4-
292
5
161
8.
64
IO.
05
14
.10
16
"
4-
975
6,
088
IO.
03
12.
01
15
•35
17-
80
5-
652
7
IO.
80
12.
94
16
.07
18.
89 " +(K2C204)2H2C204.2H20
6.
27
7.
87
ii.
47
14.
13
16
•Si
19.
59 (K2C204)2.H2C204.2H20
7-
63
9
,72
12.
16
15-
ii
16
.80
20.
IO
8.
66
ii
14
12.
32
15-37
16
•95
2O.
34
9-
055
ii
58
12.
90
16.
23
17
.14
20.
70 " +K2Q04.H20
8.
826
ii
52
12.36
16.
14
16
2O.
41 KzC-A-HijO
5-
215
12,
33
8.52
15.
03
15
•94
2O.
II "
2.
23
14
,80
4-
53
«$•
55
15
.06
19.
66
I.
245
16
,82
I.
87
18.
17
8
.82
19.
2S
0.
871
18
4
0.
74
22.
32
2
.04
23-
09
0.
511
20
91
.
0
•434
29
"
0.
325
23
30
0
.365
31-
40
0
4i
3t
O
4o!
79
O
51-
34 KOH.H2O
* Supersaturated.
t
About.
EQUILIBRIUM IN THE SYSTEM POTASSIUM OXALATE, OXALIC ACID, WATER
AT 25°.
Gms.
er 100 Gms.
it. Sol.
(Hartley, Drugman, Vlieland and Bourdillon, 1913.)
Solid Phase.
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
Q03.
K20. '
3-079
2.052
KH3(Q04)2.2H20
3-450
2.360
" +KHCA
3-793
3-199
KHCA
5-457
5-9I9
"
9.816
11.96
" +2K2C2O4.H2C2O4.2H2O
12.365
15.71
2K2QO4.H2CzO4.2H2O +K2C2O4.H2O
11-85
I5-5I
K2C2O4.H2O
QO,. K,0.
8.29 o
8.278 0.045
7.412 0.064
2.827 0.238
2.007 0.346
1-734 0.567
2.675 I.7H
Similar data at 15° for the above system are given by .Jungfleisch and Landrieu
55i
POTASSIUM OXALATES
SOLUBILITIES IN THE SYSTEM POTASSIUM OXALATE, OXALIC ACID, WATER AT
THE CRYOHYDRIC POINTS.
(Koppel and Cahn, 1908.)
(Temp, of Equilibrium of Solution with Ice.)
teoflce
Separa-
tion.
— 0.9S
— 0.90
-0.52
-0.25
— 0.58
— 0.78
-1.50
— 2.10
-2.78
-345
Gms. per 100
Cms. Sat. Sol.
Solid Phase,
Ice+:
H2C204.2H20
" +KH3(CA),.2H2O
KH3(CA)2.2H20
<<
" +KHCA
KHCA
" +(K2CA;2.
H2CA.2H20
t° of Ice
Separa-
tion.
- 4-45
- 5-20
- 5.32
- 5.97
- 6.55
— 8.10
— 10.30
— 13.60
— 17.40
-23.80
Gms. per 100
Gms. Sat. Sol.
Solid Phstee,
Ice+:
;K2CA)2.H2CA.2H20
" -f-K2C204.H20
K2CA.H,0
«i
«
«
u
CA
2.641
2.720
1.672
0.643
1.229
1.648
2.707
3.687
4.576
5-681
K20.
0.0466
0.0602
O.2IO
0.823
1.234
2.950
4.363
5-50
7-05
CA
6.902
7.616
7.696
8.51
6.742
4-999
3.358
1.854
i. 200
0.606
K20. '
8.820 (
9-74
9.84
II.OI
10.45
10.86
11.76
13.08
14.55
16.89
SOLUBILITIES IN THE SYSTEM POTASSIUM OXALATE, OXALIC ACID, WATER AT
THE BOILING POINTS.
(Koppel and Cahn, 1908.)
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
KH3(CA)2.2H20
"+KHCA
KHCA
CA. K20.
39.84 5-25
36.95 5.83
32.75 5-97
27.64 9.12
27.46 11.43
23.36 10.50
18.81 12.29
t°of
B.pt.
Gms. per 100 Gms.
Sat. Sol.
'CA. K2o. '
102.8
19.10 18.25
103.25
21. II 21.71
107.7
25.19 27.91
106.35
22.04 26.45
106.25
19.17 25.02
108.25
12.73 27.69
iii.S
5-35 30.40
Solid Phase.
KHCA
" +K2C204.H20
K2CA.H20
t°of
B.pt.
105.5
104.9
104.3
103.4
102.9
102.5
102.4
From the preceding tables the following results for the solubilities of the
pure oxalates in water are obtained.
SOLUBILITY OF POTASSIUM OXALATE, K2C2O<.H2O IN WATER.
t°
Gms. per 100 Gms
Sat. Sol. Solid
A0 Gms. per
roo Gms. Sat. Sol. Solid
If
CA + K2O =
K2CA. Phase-
C A + K20 =
=K2CA- phase-
— 0.78 1.31
1.71
3.02 Ice
30
12.36
16.14
28.50 K2C204.H20
— I
49
2.48
3-20
5-68 "
40
13.20
17.22
30.44
— 2
•50
3-99
5.20
9-195 "
50
14.14
18.46
32.60
- 3
.22
5-iS
6.705
11.855 "
60
15.06
19.66
34.72
- 5
.88
8.429
II.OI
19.43 " +K2CA-H2O
70
15-94
20.81
36.75
o
8.83
11.52
20.35 K2CA.H2O
80
16.86
22.02
38.875
+ 10
10.48
13.69
24.17
90.2
17.73
23.14
40.90
20
11-57
15.11
26.675
106.2*
19.17
25.02
44.19
* b. pt.
100 gms. sat. aq. sol. contain 20.62 gms. K2C2O4 at o°, d = 1.161. (Engel, 1888.)
The results oL Hartley, Drugman, Vlieland and Bourdillon (1913) and of
Colani (1916), for the solubility of neutral potassium oxalate in water, agree
satisfactorily with the above.
SOLUBILITY OF POTASSIUM BIOXALATE, KHC2O4, IN WATER.
(Koppel and Cahn, 1908.)
t°. Gms. per zoo Gms. Sal Sol, j^ phase.
C2Oj. K2O.
60 8.75 6.50 KHCA
I02.4b.pt. 18.81 12.29 "
The KHC2O4 is decomposed to the less soluble tetroxalate at temperatures
below 50°.
POTASSIUM OXALATES
552
SOLUBILITY OF POTASSIUM TETROXALATE, KH3(C2O4)2.2H2O, IN WATER.
(Koppel and Cahn, 1908.)
— o. 25 cryohydrate
o
30
60
103.5 b. pt.
Gms. KH3(C2O4)2 per
100 Gms. H2O.
0..99
1.27
4-30
n-95
72.17
Solid Phase.
SOLUBILITY OF MIXTURES OF POTASSIUM OXALATE AND OTHER SALTS IN
WATER. (Coiani, 1916.)
Results at 15°.
Gms. per 100 Gms. Sat. Sol.
Results at 50°.
Gms. per too Gms. Sat. Sol.
Solid Phase in
Each Case.
K2C2O4.H2O+KC1
10.03 K2C2O4+i9.i9 KC1 15.18 K2C2O4+2o.26 KC1
23.55 " + i.82K2SO4 31.06 " + i.99K2SO4
20.39 +11.60 KNO3(i9°) 19.63 +28.29 KNO3 " +KNO,
ipo gms. aqueous solution, simultaneously saturated with potassium and
sodium oxalates, contain 26.15 gms- K2C2O4 + 2.44 gms. Na2C2O4 at 25°.
(Foote and Andrew, 1905).
POTASSIUM Telluric Acid OXALATE K2[HdTe06.C2O4].
(Rosenheim and Weinheber, 1910-11.)
SOLUBILITY IN WATER.
t°
Gms. K2[H6TeO6.C2O4] per 100 gms. H2O
POTASSIUM PERMANGANATE KMnO4.
SOLUBILITY IN WATER. (Baxter, Boylston, and Hubbard, 1906; Patterson, 1906.)
O
2.67
2O
5.36
6.82
4o~
9.07
5o°
12.35
Gms. KMnO4 per 100:
Gms. KMnO4 per 100 :
I .
Gms. Solution.
Gms. H2O.
cc. Solution (P).
o
2-75
2.83
2.84
9.8
4-31
15
. . .
5-22
19.8
5-96
6-34
24.8
7.06
7-59
. . .
29.8
8.28
9-03
8.69
Gms. Solution.
Gms. H2O.
34-8
i 9.64
10.67
40
ii. 16
12.56
45
12.73
14.58
50
14-45
16.89
55
16.20
19.33
65
20.02
25.03
Sp. Gr. of saturated solution at 15° = 1.035.
Determination by Worden (1907), made with extreme care, gave results in
very close agreement with the above.
SOLUBILITY OF POTASSIUM PERMANGANATE IN:
Water.
(Voerman, 1906.)
Aqueous Acetone Solutions at 13°.
(Herz and Knoch, 1904.)
Gms. KMn04 per 100 Gms.
cc. Acetone
KMn04 per 100 cc. Solutit
A
'
Solution.
Water.
per 100 cc.
Solvent.
Millimols. Grams.
— 0.18
0.58
0.58 Ice
0
148.5
4.70
- 0.27
0.99
I.OI "
10
162.5
5.13
- 0.48
1.98
2. 02
20
177-3
5-61
- 0.58
2.91
3 Ice+KMnO
30
208.2
6.59
+10
4.01
4.22 KMnO4
40
257-4
8.14
15
4-95
5-20
50
289.7
9.16
25
7
7-53
60
316.8
10. 02
40
10.40
ix. di
70
328
10.38
So
14-35
16.75 "
80
312.5
9.89
90
227
7.18
100
67
2.14
553 POTASSIUM PERMAN-
GANATE
SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS OF
POTASSIUM CARBONATE.
(Sackur and Taegener, 1912.)
Mols. KMnO4 per Liter in:
t°.
O.I ft ^ivjCAJg.
i n |K2CO3.
2 n £K2CO3.
4 n iK2C03.
6 n iK2C03.
0
o. 1462
0.0629
o . 0446
0.027
0.0156
25
0-4375
0.2589
. . .
0.093
40
0.7380
0.5007
0.3519
... v
SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS OF
POTASSIUM CHLORIDE.
(Sackur and Taegener, 1912.)
Mols. KMnO4 per Liter in:
t°.
o.i « KC1.
0.5 n KC1.
i n KC1.
2 n KC1.
o
0.1395
0.076
0.0532
0.0379
25
0.4315
0.306
0.220
0.1432
40
0.738
0.584
0.444
0.288
SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS OF
POTASSIUM HYDROXIDE.
(Sackur and Taegener, 1912.)
Mols. KMnO4 per Liter in:
t°. H2O.
i » KOH.
2 « KOH.
4 »
KOH.
6«
KOH.
8 n KOH. 10 n KOH.
0
0
. 176
0.050
0
.031
0.
027
O
023
O.OI7
O.OI2
10
o
,278
O. 112
0
.068
0.
048
0
.042
0.028
0.016
20
0
,411
0.179
o
.119
0.
079
o
.074(19°)
0.032
0.029
30
0,
573
0.316(32°)
o
.213(32°)
0.
149(32°)
0.
114
0.062(32°)
0.040
40
o,
792
0-439
0
.306
0.
211
0
,161
0.084
0.052
50
I ,
154(53°)
0.638
0
.462
0.
304
0
.219
O.III
. . .
70
I.
812
I.I72
0,
869
0.
572
o
390
0.188
0.082
80
I-5I3
I.
190
0,
500
0.231
. . .
90
. . .
. . .
0,
649
0.297
SOLUBILITY OF POTASSIUM MANGANATE IN AQUEOUS SOLUTIONS OF
POTASSIUM HYDROXIDE.
(Sackur and Taegener, 1912.)
(The KzMnO* was prepared by boiling KMnO4 with very cone. KOH, draining
by suction and washing with ice cold K2CO3 solution. The impurities were of
no consequence since the determinations were made in alkaline solutions.)
Mols. K2MnO4 per Liter in:
O
10
15
20
30
40
45
50
60
70
80
2 n KOH.
4 n KOH.
6 » KOH.
8 n KOH.
10 n KOH.
0.907
0-554
0.155
0.063 •
0.0145
I.OI3
. . .
0.07O
0.0152
. . .
0.681 (17°)
0.224
. . .
I.I4O
0-733 (2S°)
0.26l (23°)
0.078
0.0160
1.252
0.772
0.303
0.096
0.0215
. . .
0.852
0.362
o. 119
0.0305
1.424
0.889
0.388
0.938 (51°)
o. 142
0.0462
1.003
0.469
0.167
0.062 (63°)
1.074
0.528
0.196
0.070
1.143
0.587
O.222
0.083
TOO cc. anhy. hydrazine dissolve 2 gms. KMnC>4, with evolution of gas and for-
mation of a brown precipitate, at room temp. (Welsh and Broderson, 1915.)
POTASSIUM PERMAN-
GANATE
554
SOLUBILITY OF
MIXED CRYSTALS OF POTASSIUM PERMANGANATE AND
POTASSIUM
PERCHLORATE AT 7°.
(Muthmann and Kuntze
, 1894; recalculated by Fock,
1897.)
MUligram Mols.
per Liter.
KC103."
Cms. per Liter.
Mol. per cent
KMnO4 in
* Crystals of Solid
Phase.
KMnO4.
KMnO4. KC1O4.
O
63.91
o 8.86
0
29-37
54.48
4-65 7-55
2.84
67-73
42.75
10.71 5-93
9.78
79.04
39-59
12.50 5.49
10. 8 1
99.81
38.63
15-79 5-36
15.96
122.24
34-39
19-34 4-77
23-56
119.21
38.91
18.84 5.39
24.28
128.08
33-77
20.26 4.68
26.40
144.46
33-14
22.86 4.59
34-32
167.81
29-53
26.55 4.09
44.42
183.09
25-I9
28.97 3.49
67-33
197.82
20. 16
. 31.30 2.80
77-95
233-75
28.26
36.98 3.92
94-37
264.27
o
41.81 o
IOO
SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM PERMANGANATE AND
RUBIDIUM PERMANGANATE AT 7°.
(Muthmann and Kuntze, calc. by Fock.)
Milligram Mols. per Liter.
Cms, per Liter.
KMn04.
27.04
75
120.26
188.30
198.36
205.76
225.12
264.27
22.69
22.22
3L29
38-98
41.29
42.50
26
o
KMnO4.
4-28
11.84
I9.03
29.80
31.39
32.56
35.6l
41.81
4.64
4-54
6.40
7.97
8.44
8.69
5.32
o
3.50
13-75
34.29
71.45
92.50
99.47
99.32
ioo
POTASSIUM PICEATE C6H2(NO2)3OK.
Data for the solubility of potassium picrate in aqueous solutions of ethyl
alcohol, methyl alcohol and of acetone at 25° are given by Fisher (1914).
POTASSIUM PHOSPHATES
SOLUBILITY OF POTASSIUM ACID PHOSPHATE, KH2PO4.H3PO4, IN WATER.
(Parravano and Mieli, 1908.)
Determinations by Synthetic (sealed tube) Method.
Gms. Gms.
Solid Phase.
t'.
Sat. Sol.
-o.6
3-337
-2.5
12.13
-6.7
29-43
- 9-2
36.98
— i3 Eutec.
44
o(?)
45-8
+ 10.9
50-3
Solid Phase.
Ice
Sat. Sol.
65.2
68.44
78
72.43
87-5
77-6
105.5
85-9
+KH2PO4
120 tr. pt.
92.1
KH2PO4
135
96. i
«
139
IOO
KH2PO4
+KH2PO4.H3PO<
One liter of sat. aq. solution contains 249.9 gms. KH2PO4 at 7°.
(Muthmann and Kuntze, 1894.)
555
POTASSIUM PHOSPHATES
SOLUBILITY OF POTASSIUM ACID PHOSPHATE, KH2PO4.H3PO4, IN ANHYDROUS
PHOSPHORIC ACID.
(Parravano and Mieli, 1908.)
Determinations by Synthetic (sealed tube) Method.
• Gms. per 100 Cms. Sat. Solution.
KH2P04.H3P04 ^ KH2P04.
38.5 18.17 10.56
84 58-42 33-97
no 77.53 45.08
126.5 92.26 S1^0
EQUILIBRIUM IN 'THE SYSTEM POTASSIUM HYDROXIDE, PHOSPHORIC ACID,
WATER AT 25°.
(D'Ans and Schreiner, igioa; Parker, 1914.)
The results of these investigators agree satisfactorily when plotted on cross-
section paper. The following figures were read from the curves. Some uncer-
tainty exists in regard to the solid phase in contact with some of the solutions.
K.
P04.
-» OU11U -T1JCI.SC.
9.62
0
KOH.2H2O
9.76
0.24
" +K3PO4.3H2O
9-15
o-5
K3P04.3H20
8.2
i
"
7-5
i-5
"
8.2
2
«
7-5
2-5
«
8.8
2.9
«
9-7
2.9
" +K3P04
9-5
3
K3P04
8-5
3-4
"
8
3-6
H
7-5
3-75
"
Fusion-point data for KPOs +
(1908, 1910).
POTASSIUM HYPOPHOSPHATE, etc.
SOLUBILITY IN WATER.
(Salzer — Liebig's Ann. 211, i, 82.)
K.
P04.
-» aoua rnase.
7
4
K3P04+K2HP04
6
3-6
K2HP04
5
3.15
"
4
2.65
" or KH2P04(?)
3
2.2
(?)
2
1-7
" " (?)
I .5
1-5
" " (?)
1.6
2
KH2PO4
2.1
4
"
2-5
6
"
3
8
"
1.65
6
KH2P04.H3P04 (Parker)
*-35
8
« «
are given
by Parravano and Calcagni
Salt.
Formula.
Gms. Salt per 100
Gms. H2O.
Cold.
400
20O
33
66.6
Hot.
Potassium Hypophosphate K4P2O6.8H2O
" Hydrogen Hypophosphate K3HP2O6.3H2O
Di Hydrogen Hypophosphate K2H2P2O6.3H2O
" Tri Hydrogen Hypophosphate KH3P2O6
" Penta Hydrogen Hypophosphate K3H5(P2O6)2. 2H2O 40
" Hydrogen Phosphite KH2PO3 172 (20°) . . .
" Hypophosphite KH2PO2 200(25°) 333
« Hypophosphite KH2PO2* 14.3 (2S°) 28
* Solvent alcohol.
IOO
200
125
POTASSIUM PHOSPHOMOLYBDATE K3PO4.iiMoO3.i|H20.
100 gms. H2O dissolve 0.0007 gip. at 30°.
100 gms. aqueous 10% HNO3 dissolve 0.204 Sm- at 3°°'
(Donk, M. G., 1905.)
POTASSIUM SELENATE 556
POTASSIUM SELENATE K2SeO4
SOLUBILITY IN WATER.
t°. -20°. -S°. +5°. 18". 97°.
Cms. K2Se04 per 100 gms. solution 51.5 51.7 52 52.6 54.9
(Etard, 1894.)
100 gms. H20 dissolve 115 gms. K2SeO4 at 12°. (Tutton, 1907.)
POTASSIUM SILICATE K2SiO3.
Data for equilibrium in the systems K2SiO3 + H2O, K2Si2O5 + H2O, K2SiO3 +
SiO2, SiO2 + H2O and K2SiO3 + SiO2 + H2O, at temperatures between 200° and
1000° +, determined by the " hydrothermal quenching method," are given by
Morey (1917).
POTASSIUM STANNATE K2SnO3.3H2O.
100 gms. H2O dissolve 106.6 gms. at 10°, and 110.5 Sms. at 20°. Sp. Gr. at
10° = I.6l8 at 20° = 1.627. (Ordway, 1865.)
POTASSIUM SULFATE K2SO4.
SOLUBILITY IN WATER.
(Mulder; Andrae, 1884; Trevor, 1891; Tilden and Shenstone, 1884; Berkeley, 1904; see also Etard, 1894.)
Gms. K,SO4 per 100 Gms. ^0
Gms. K2SO4 per 100 Gms.
Gms. K2SO4
per loo Gms.
'
Water.
Solution.
Water.
Solution.
*
Water.
Solution.
0
7-35
6.85
40
14.76
12.86
90
22.8
18-57
10
9.22
8.44
50
16.50
14.16
IOO
24.1
19.42
20
II .11
IO
60
18.17
I5-38
I2O
26. $
20.94
25
I2.O4
10-75
70
19-75
16.49
143
28.8
22.36
30
12.97
11.48
80
21.4
17-63
170
32.9
24.76
Sp. Gr. of solution saturated at 18° = 1.083.
The determinations of Berkeley (1904), which were made with exceptional care,
are as follows:
^.0 Sp. Gr. of Sat. Gms. K2SO4 per f „ Sp. Gr. of Sat. Gms. K2SO4 per
Solution. loo Gms. H2O. Solution. 100 Gms. H2O.
0.40 ' 1.0589 7.47 58.95 1.1089 iS.OI
15.70 1.0770 IO-37 74-85 I.II57 20.64
31.45 I.092I 13.34 89.70 I.II94 22.80
42.75 i.ioio 15.51 ioi.ib.pt. 1.1207 24.21
Individual determination in good agreement with the above, are given by Le-
Blanc and Schmandt (1911); Greenish and Smith (1901); Osaka (1903-8); Nacken
(1910); Smith and Ball (1917).
SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM SULFATE AND AMMONIUM
SULFATE AT 25°.
(Fock, 1897.)
Grams
per Liter.
Milligram Mols. per Liter.
Mol. per cent Sp. Gr.
K2SO4 in of
Solution. Solution.
Mol. per cent
K2SO4 in
Solid Phase.
' KaSCV
(NH4)2S04.
K2S04.
(NH4)2S04. '
127-9
o.o
734
O-O
IOO
1. 086
IOO
135-7
"5-7
778.5
874.6
47-1
1.149
91.28
84.20
28l.I
483
2126
I8.5
1 .200
80-05
59.28
355-o
340
2685
11.13
1 .226
68.63
40.27
482.7
231
3650
5-98
1 .246
27-53
o.oo
542-3
o.o
4100
0-00
1.245
0-00
Results are also given for 14°, 15°, 16°, 30°, 46°, and 47°.
557
POTASSIUM SULFATE
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS AMMONIA SOLUTIONS AT 20°.
(Girard, 1885.)
Cms. NH3 per ioo cc. solution o 6.086 15.37 24.69 31.02
Gms. K2SO4 per loo cc. solution 10.80 4.10 0.83 0.14 0.04
One liter sat. solution in water contains 105.7 Sms. K2SO4 at 20°.
One liter sat. solution in 5.2% NH3 contains 45.2 gms. K2SO4 at 20°.
(Konowalow,
SOLUBILITY DATA FOR THE RECIPROCAL SALT PAIR
K2SO4 + BaCO3 <=* K2CO3 + BaSO4.
(Meyerhoffer, 1905.)
25
25
80
80
80
IOO
IOO
Gms. per ioo Gms.
t8.
Sat. Sol.
Solid Phase.
K2S04.
K2C03.
25
10.76
O
K2SO4+BaS04
25
6.76
5-85
" "
25
3-92
12.6
<< ««
25
2.485
17.81
"+BaC03
25
1.72
22.1
K2SO4+BaCO3
25
0.0886
28.5
« «
25
0.023
53-i
" +K2C03.2H20
25
O
53-2
K2CO3.2H2O+BaCO3
Gms. per ioo Gms.
Sat. Sol.
Solid Phase.
K2S04.
K2C03.
O.6O2
7-35
BaC03+BaS04
0.173
2.85
"
0.613
2.49
"
i-39
4.88
"
7-i
15-33
"+K2SO<
0-797
2-36
BaC03+BaS04
1.83
4-5i
"
9.42
13-6
" +K2S04
SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM COPPER SULFATE AND
AMMONIUM COPPER SULFATE IN WATER.
CuS04.K2SO4.6H2O and CuSO4(NH4)2SO4.6H2O at I3°-I4°.
(Fock, 1897.)
Mols. per ioo Mols.
H20-
Mol.
per cent K Salt.
Mols. per too Mols.
H20.
Mol. per cent K Salt.
K
O
0.
0.
o.
. Salt.
0897
2269
2570
NH4 Salt.
1-035
0.8618
o . 6490
0.5887
in Solution
0
5.06
16.76
30.40
. in Solid.
0
10.34
33-05
46.22
K Salt.
o . 2946
0-3339
0.4560
0-4374
NH< Salt.
o . 5096
0.3319
0.1961
0
in Solution.
36.63
50.15
69-93
IOO
lin Solid.
58.20
75-34
83.86
IOO
SOLUBILITY OF SOME POTASSIUM DOUBLE SULFATES IN WATER AT 25°.
(Locke, 1902.)
Gms. Anhydrous Salt
per ioo Gms. H2O.
12.88
Double Salt.
Potassium Cobalt Sulfate
Copper "
Nickel
Zinc
Formula.
K2Co(SO4)2.6H2O
K2Cu(SO4)2.6H2O
K2Ni(S04)2.6H20
K2Zn(SO4)2.6H2O
II .69
6.88
SOLUBILITY OF POTASSIUM NICKEL SULFATE AND ALSO OF POTASSIUM ZINC
SULFATE IN WATER, EACH SEPARATELY DETERMINED AT DIFFERENT TEM-
PERATURES.
o
10
20
25
30
Gms. per ioo Gms. H2O.
.6H2O.
6
9
14
16
18
13
19
26
30
35
t8.
40
50
60
70
Gms. per ioo Gms. H2O.
23
28
35
43
45
56
72
88
POTASSIUM SULFATE 558
SOLUBILITY OF THE THREE HYDRATES OF POTASSIUM FERROSULFATE
IN WATER AT DIFFERENT TEMPERATURES.
(Kuster and Thiel, 1899.)
KgSCU.FeSp4.6H2G-. K2SO4.FeSO4.4H2O. K2SO4.FeSO4.2H2O.
t«. cc.N/ioKMnO4 Cms. K2SO4 cc.N/ioKMnO4 Gms.K2SO4 cc.N/ioKMnO4 Gms.K2SO"
per 2cc.
Solution.
.FeSO4 per
100 cc. Sol.
per 2 cc.
Solution.
.FeSO4 per
100 CC. Sol.
per 2 cc.
Solution.
.FeSO4 per,
100 cc. Sol.4
o-5
12-4
18.36
*S'S
22-94
15-4
22-79
17.2
17.0
25.16
18.1
26.79
21 .6
3I-98
40.1
24.8
36.72
21.9
32.41
27.6
40-86
60
29.0
42-93
24.1
35-68
28.8
42.63
80
30.6
45-29
27-3
40.46
28.6
42-34
90
. . .
29.6
43-82
28.9
42-73
95
...
29.8
44.11
27.7
41 -or
SOLUBILITY OF MIXTURES OF POTASSIUM AND LEAD SULFATES AND OF
POTASSIUM AND STRONTIUM SULFATES IN WATER.
(Barre, 1909.)
Results for K2SO4 + PbSO4. Results for K2SO4 + SrSO4.
Cms. K2SO4 Cms. K2S04
t°. per zoo Cms. Solid Phase. t°. per 100 Cms. Solid Phase.
Sat. Sol. Sat. Sol.
7 0.56 PbS04.K2S04 17.5 1.27 K2S04.SrS04+SrSO<
17 0.62 " 50 1.88 "
50 1.09 " 75 2.71
75 i-37 ioo 3.90
100 1.69
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE, BROMIDE, AND IODIDE.
(Blarez, 1891.)
Interpolated from the original results.
Grams K2SO4 per too cc. in Aq.
Grams Halogen Solutions of:
Salt per 100
cc. Solution.
O
2
4
6
8
10
12
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM
HYDROXIDE AT 25°.
(D'Ans and Schreiner, 1910.)
KC1
KBr
KI
at 12.5°.
at 14°.
at 12.5°.
9.9
10. 16
9-9
8-3
9.1
9-2
7.0
8.2
8.4
5-7
7-4
7-7
4.6
6.6
7-2
3-5
6.0
6.6
5-5
6.0
Mols. per 1000 Cms.
Sat. Solution.
Gms. per 100 Cms.
Sat. Solution.
Mols. per 1000 Gms.
Sat. Solution.
Gms. per 100 Gms.
Sat. Solution.
(KOH)2.
0
0.258
0-433
I-I3
K2S04.'
0.6l7
0-433
0.280
0.137
KOH.
O
2.892
4.854
12.67
K2S04.
10-75
7-544
4.878
2.386
(KOH)2.
2.86
3-42
4.809
K2S04.
0.035
0.009
0
' KOH.
32.06
38.33
53-51
K2S04.
0.61
0.16
o
559
POTASSIUM SULFATE
SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM SULFATE AND POTASSIUM
CHROMATE AT 25°
(Fock, 1897.)
Milligram
Mols. per Liter
Grams per Liter.
Mol. pe
:r cent Sp. Gr. Mol. per cen?
r\ ;., — £ v o/-\ •
' K2S04.
K2Cr04.
K2S04.
K2Cr04:
K2So4 iu ui
Solution. Solution.
J\.2O^4 HI
Solid Phase.
618
i
O
• O
107
•7
O
.00
100
.0 1-083
IOO.O
608
4
103
106
.0
2O
.02
85
.51 1.092
99.65
34i
.0
691
.8
59
.46
134
•5
33
.01 1.141
97-30
174
.8
1496
.0
30
•47
290
•5
10
•50
.231
91.97
no
•7
2523
19
•30
49°
•5
4
.21 3
•356
28.43
100
.6
2687
17
•54
522
•3
3
.60
•377
2-41
0
0
2847
0
.0
553
•5
0
• OO
•398
o.oo
734
-O
O
.0
127
•9
0
.0
100
•O 3
.0863
IOO.O
617
.0
103
•4
107
.6
20
.1
85
.65 3
•0934
99.78
463
452
•7
80
.72
88
.0
55
•55
•I235
98.49
279
948
.2
48
.64
184
•4
22
.72 1.1700
96.07
1469
26
.68
285
.6
9
.41 1-2255
85-77
296
268l
51
.61
521
.2
21
.09 1.3688
25-73
o
.0
2715
0
.00
527
.8
0
.00 1-3781
o.oo
SOLUBILITY OF POTASSIUM SODIUM SULFATES IN WATER.
Double Salt.
3K2S04.Na2SO4
5K2SO4.Na2SO4
103-5
4-4
12.7
100
Gms. per 100
Cms. H2O.
Authority.
40.8
(Penny, 1855.)
9.2
(Gladstone, 1854-)
10. 1
25
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
SULFATE.
Results at 25°.
(Smith and Ball, 1917.)
Gms. per 100 Gms.
Results at 34° and at 6o°-
(Nacken, 1910.)
Na2S04.
O
I.78
3-58
5.38
7.19
K2S04.
12.05
12-33
12.65
12.89
13.12
Gms. per 100 Gms.
Sat. Sol. at 34°-
Gms. per 100 Gms.
Sat. Sol. at 60°.
Solid Phase
at 34° and at 60°.
Na2SO4.
K2so4:
'Na2S04.
K2S04.
0
11.9
0
15-3
K2S04
7.1
10.7
6.6
13-9
" +Glaserite
31-4
4.3
27.1
8.2
NajSC^+Mix crystals
33 • I
0
0
NajS04
Additional data for the above system at 15°, 25°, 40°, 50°, 60°, 70° and 80° are
given by Okada (1914). The results show that potassium and sodium sulfates
form a double salt of the composition "K3N a (SO4)2. This double salt dissolves
sodium sulfate as a solid solution but not potassium sulfate.
POTASSIUM SULFATE 560
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 1 8°.
Mols. per 100 Mols.
K2S04+H2SQ4+H20.
K^SOT H2S04.
I. 10 O
i-59 o-95
2.49 2.70
2-75 3-17
2-75 3-74
2.83 5.08
(Stortenbecker, 1902.)
Solid Phase.
K2S04
Mols. per 100 Mols.
K2S04+H2S04+H2O.
K2S04.
2.80
2.61
2. 25
I. 08
0.77
0.44
H2S04.
5-79
5-6i
6. 19
7-94
9.2
22.7
Solid Phase.
K2SO4.3KHSO4
K2SO4.6KHSO4
" +KHS04
KHS04
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT o°.
(D'Ans, igoga.)
Mols. per 1000 Cms.
Sat. Sol.
K2S04. H2S04.
0-53 <
0.64 <
0.74
5-37
3-75
.08
0-73
•13
0.71
0.69
0.69 :
•44
.66
.88
Solid Phase.
K2S04
" +K3H(S04),
+Ka
SS.
Sol.
K2S04.
0.61
0-54
o-53
0-43
0.28
O.I2
0.09
H2S04.
2.12
2.29
2.30
2.48
3-04
4-43
5-27
Solid Phase.
Ka+Kb
Kb
" +KHS04
KHSO4
Ka and Kb are acid sulfates between K3H(SO4)2 and KHSO4. Their composi-
tions were not determined.
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 25°.
(D'Ans, igoga, igia; see also Herz, ig 11-12.)
Mols. per 1000 Gms.
Sat.
Sol.
Solid Phase.
K2S04.
H2SO4. '
.27
I-3I
K2S04+K3H(S04)2
•33
1.99
K3H(S04)2+Ky
.24
2.03
Ky
•13
2.17
"
.04
2-35
" +KHSO4
.032
2-345
KHS04
0.67
2.83
«
O.22
4-13
"
0.15
5.36
«
K2S04.
H2SO4+SO3.
O.I7I
6.42
KHS04
O.I90
6.60
«
0.266
0.182
6.91
7.26
" +KH3(SO4)2.H2O
0.157
7.62
0.167
7-88
0.201 8
Ky = an acid sulfate between
position was not determined.
Mols. per 1000 Cms.
Sat. Sol.
Solid Phase.
K2SO4.
H2S04+S03.
0.250
8.10
KHsCSO^.HzO
0.352
8.15
"
0.364
8.16
" -l-KHaCSOO,
0.341
8.29
KHsCSO,),
0.322
8.33
"
0.325
8-45
"
0.346
6.62
«
0.384
8-57
«
0.412
8.71
K
0.583
8.82
«
0.880
8.65
" +KHS207
0.899
8.63
KHS207 (unstable)
0.882
8.70
«
0.561
8.96
"
0.365
9.80
"
0-43
9-78
(i
0.665
9.80
"
0-937
9.66
«
and KHSO4 of which the exact com-
56i POTASSIUM SULFATE
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS ALCOHOL.
(Gerardin, 1865; Schiff, 1861.)
In Aq. Alcohol of 0.939 In Alcohol of Different
Sp. Gr. = 40 Wt. %. Strengths at 15°.
,0 Cms. K2SO4 per ioo Weight per Cms. K2SO4 per too
Cms. Alcohol. cent Alcohol. Cms. Sat. Sol.
40 0.16 10 3.90
80 O.2I 2O 1.46
60 0.92 30 0.56
40 0.21
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS ALCOHOL AT 25°.
(Fox and Gauge, 1910.)
Cms. per ioo Gms. Sat. Solution. Cms. per ioo Cms. Sat. Solution.
K2SO4. C2H5OH. H20. K2SO4. C2H5OH. H2O.
9.17 1.35 89.48 2.66 15.26 82.08
6.90 4.80 88.30 1.83 20.50 77-67
4.96 7.80 87.24 0.97 26.91 72.12
4.32 9.70 85.98 0.41 35.97 63.62
3.57 12.34 84.09 0.22 43.90 55.88
2.71 14.51 82.78 0.016 69.26 30.72
SOLUBILITY OF POTASSIUM SULFATE AT 25° (Fox and Gauge, 1910.) IN:
Aqueous Chloral Hydrate Solutions. Aqueous Glycerol Solutions.
Gms. per ioo Gms. Sat. Solution. Gms. per ioo Gms. Sat. Solution.
K2S04. CC13CH(OH)2. H2O. K2SO4. (CH2OH)2CHOH. H2O.
9.13 6.44 84.43 8.87 8.96 82.17
8.41 9.09 82.50 7.69 13-36 78-95
7.79 12.38 79.83 6.47 20-34 73.19
7.31 13.20 79.49 5.83 24.15 70.02
5.88 22.07 72.05 4.44 33.73 61.83
4.54 33.15 62.31 3.65 40.40 55.95
3.36 44.40 52.24 3.38 43.52 53.10
2.92 47.30 49.78 2.69 50.18 47.13
2 62.82 35-i8 2.07 57-22 40.71
1.75 70.28 27.97 i-53 67.94 3°-53
1.40 80.36 18.24 0.98 78.18 20.84
i. 08 85.26 13.66 0.73 98.28 0.99
SOLUBILITY OF POTASSIUM SULFATE AT 25° (Fox and Gauge, 1910.) IN:
Aqueous Acetone Solutions. Aqueous Pyridine Solutions.
Gms. per ioo Gms. Sat. Solution. Gms. per ioo Gms. Sat. Solution.
K2SO4. (CH3)2CO. H2O. K2SO4. CH<(CH.CH)2>N. H2O.
7.20 4.92 87.88 7.95 4.23 87.82
5.02 10. 06 84.92 4.77 13.90 81.33
2.96 16.23 8o.8l 2.75 24.51 72.74
1.50 24.31 74.19 1.47 34.19 64.34
0.47 37.19 62.34 0.45 46.29 53.26
0.20 46.29 53.51 0.12 55.93 43.95
0.03 62.40 37-57 0.006 75-QO 24.09
POTASSIUM SULFATE 562
SOLUBILITY OF POTASSIUM SULFATE AT 25° (Fox and Gauge, 1910.) IN:
Aqueous Ethylene Glycol Solutions. Aqueous Mannitol Solutions.
Gms. per 100 Gms. Sat. Solution. Gms. per 100 Gms. Sat. Solution.
K2S04. (CH2OH)2. H20. K2S04. (CHOH)4(CH2OH)2. H2O.
9.67 3.16 87.17 10.32 3.20 86.48
7.69 9.79 82-53 9-61 8-35 82.04
5.74 18.47 75.79 9.19 11.26 79.55
3.57 32.11 64.32 8.66 14.30 77.04
1.83 49-°3 49-14 8.35 17.22 74.43
SOLUBILITY OF POTASSIUM SULFATE AT 25° IN:
Aq. Sucrose Solutions. Aq. Potassium Acetate Solutions.
(Fox and Gauge, 1910.) (Fox, 1909.)
Gms. per 100 Gms. Sat. Solution. Gms. per 100 Gms. Sat. Solution.
K2S04. CuHaOu. H20. K2SO4. CH3COOK. H2O.
9.65 9.56 80.79 6.65 6. ii 87.24
8.65 18.55 72.80* 5.09 8.68 86.23
7.42 28.16 64.42 3.99 11.29 84.72
6.35 37.24 56.41 2.35 15.59 82.06
5.21 47.55 47.24 1.23 20.12 78.65
4.24 57 38.76 0.39 29.95 69.66
100 gms. glycerol of d = 1 .255 dissolve 1.316 gms. K2SO4 at ord. temp. (Vogel, 1867.)
SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS ACETIC ACID AND IN
AQUEOUS PHENOL SOLUTIONS AT 25°.
(Rothmund and Wilsmore, 1902.)
In Aq. Acetic Acid. In Aq. Phenol.
Mols. per Liter. Grams per Liter. Mols. per Liter. Grams per Liter.
' '
taCOOH. K2S04. CH3COOH
. lv2SO4. C-gxi^Oii. K2SC/4.
C6H5OH. K2SO,.
o.o
0-6714
0
.0
117
.0
0-0
o
.6714
0
.0
117.0
0.07
0.6619
4
.2
JI5
•4
0.032
o
.6598
3
.01
115.0
0-137
0-6559
8
.22
114
•4
0.064
o
.6502
6
.02
IJ3-3
0-328
0.6350
19
.68
no
.8
0.127
0
.6310
II
•94
no.o
0-578
0.6097
34
.68
1 06
•3
0.236
o
.6042
22
.19
I05-3
I.I5I
o-5556
69
.06
96
.87
0.308
o
•5834
28
•97
101 .7
2.183
0-4743
128
•58
82,
.70
0.409
o
•5572
38
.46.
97.2
0.464 0.5480 43 .63 95.5
0.498 (sat.) 0-5377 46.82 93.8
100 gms. water dissolve 10.4 gms. K2SO4 + 219 gms. sugar at 31.25°, or 100
gms. sat. solution contain 3.18 gms. K2SO4 + 66.74 gms- sugar. (Kohler, 1897.)
loo gms. 95% formic acid dissolve 36.5 gms. K2SO4 at 21°. (Aschan, 1913.)
100 gms. 95% formic acid dissolve 14.6 gms. KHSO4 at 19.3°.
100 cc. anhydrous hydrazine dissolve 5 gms. K2SO4 at room temp.
(Welsh and Broderson, 1915.)
100 gms. hydroxylamine dissolve 3.5 gms. K2SO4 at 17-18°. (de Bruyn, 189*.)
FREEZING-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES:
K2SO4 + K2WO4. CAmadori, 1913-)
•f Ag2SO4. (Nacken, 19070.)
+ NaCl. (Sackur, 1911-12.)
H- Na2SO4. (Jaenecke, 1908; Nacken, 1907 (b) (c); Sackur, 1911-12).
+ SrSO4. (Grahmann, 1913; Calcagni, 1912, 19124.)
563 POTASSIUM BiSULFATE
POTASSIUM BiSULFATE KHSO4.
SOLUBILITY IN WATER.
(Kremers, 1854.)
t°. o°. 20°. 40°. 100°.
Cms. KHS04 per ioo gms. H2O 36.3 51.4 67.3 121.6
See also p. 560.
POTASSIUM PerSULFATE
SOLUBILITY IN WATER.
(Tarugi, 1904.)
+o Gms. K-^Og per to Gms. K^Og per f 0 Gms. I^Og per
1 ' ioo cc. Sat. Sol. ioo cc. Sat. Sol. ioo cc. Sat. Sol.
o 1.620 15 3.140(3.7) 30 7.190(7.7)
5 2.156 20 4-490 35 8.540
10 2.600 25 5-840 40 9.890
The results in parentheses are the averages of a large number of determinations
by Pajetta (1906). This investigator employed constant agitation for various
lengths of time. Tarugi approached equilibrium from above as well as below but
stirred the solutions only at intervals. The determination of the dissolved per-
sulfate was made by boiling a measured volume of the clear saturated solution for
20 min. and titrating the H2SOi liberated, according to the equation K2S2O8-f-H2O
= K2SO4 + H2SO4 + O. Tarugi also reports that the presence of a number of
sodium and other salts in solution, does not appreciably alter the solubility of
K2S2O8 in water.
ioo gms. H2O dissolve 1.77 gms. K2S2Os at o°. (Marshall, 1891.)
SOLUBILITY OF POTASSIUM PERSULFATE IN SATURATED AQUEOUS SALT
SOLUTIONS AT 12°.
(Pajetta, 1906.)
(An excess of the salt and of K2S2O8 was, in each case, added to water and the
mixture stirred at constant temperature for 10 to 20 hours.)
Salt Gms. K2S2O8 per sl Gms. K^Og per
balt'
. .
ioo Gms. Sat. Sol. balt' ioo Gms. Sat. Sol.
Water alone 3.196 K2SO4 0.798
Na2SO4.ioH20 6.238 KHS04 0.336
NaHS04 8.842 KNO3 0.904
Na2HPO4.i2H2O 4.766 K2CO3 0.0146
Na2B4O7.ioH2O 3.825 KHCO3 0.317
NaNO3 19.302 MgSO4.7H2O 2.990
Na2CO3.ioH2O 5.682 CaSO4.2H2O 3.384
NaHC03 5.042
Additional determinations made with salt solutions of lower concentrations
than saturation, gave the following results at 12.5°.
Gms. Salt per Gms. KjSjOg Gms. Salt per Gms.
Salt. ioo Gms. per ioo Gms. Salt. ioo Gms. per ioo Gms.
H20. Sat. Sol. H2O. Sat. Sol.
Na2CO3 2.304 4.297 NaHS04 5.218 4.556
NaHCO3 3.652 4.230 NaNO3 3.696 4.613
Na2SO4.ioH2O 7 4.554 Na2HP04 3.086 4.446
POTASSIUM Ethyl SULFATE K(C2H6)SO4.
SOLUBILITY IN WATER.
(Illingworth and Howard, 1884.)
Gms. K(C2H5)SO4
t°. per ioo Gms.
Sat. Sol.
— 14.2 45.01
O 53-71
+ 15 62.35
POTASSIUM Ethyl SULFATE 564
SOLUBILITY OF POTASSIUM ETHYL SULFATE, POTASSIUM METHYL SULFATE AND
OF POTASSIUM AMYL SULFATE IN WATER, DETERMINED BY THE FREEZING-
POINT METHOD. (Ulingworth and Howard, 1884.)
Results for K(C2H6)SO4 Results for K(CH3)SO4 Results for K(C6HU)SO4
+ H2O. + H2O. + H2O.
j.o t Gms. xo -r Gms. +o'r Gms.
SSL
— 2.2 10 Ice — 2.3 10 Ice — 1.9 10 Ice
— 4.9 20 " — 3.6 15 — 4.3 20
— 8.2 30 — 5 20 — 5.4 24 "
— 12.1 40 — 8 30 " +K(C6H11)SO4
- 14.2 45 . 01 "+K(C2HB)S04 - 1 1 . 8 39 . 84 " +K(CH3)SO4 - 4-8 25 K(C6Hn)SO4
— 6 50 EXCzHjJSO* —11.5 40 K(CH3)S04 o 33-44
o 53-71 o 47.1 +17-3 59-46
+ 15 62.35 +12.3 54.8
POTASSIUM Sodium SULFITE KNa2H(SO3)2.4H2O.
100 gms. H2O dissolve 69 gms. of the salt at 15°. (Schwicker, 1889.)
POTASSIUM SULFONATES
SOLUBILITY IN WATER.
Gms. Anhy-
Salt. t°. drous Salt per Authority.
100 Gms. H2O.
Potassium Naphthalene Monosulfonate4H2O 25 8 . 48* (Witt, 1915.)
" 2 Phenanthrene Monosulfonate.-IHaO 20 0.273 (Sandquist, 1912.)
3 " " .oH20 20 0.342
10 .iH2O 20 0.84
" o Guaiacol Sulfonate (Thiocol) 15-20 16.6 (Squire & Caines, 1905.)
* d = 1.029
loocc.QOvol. % alcohol dissolve 0.25 gm.thiocolat I5°-2O°. (Squire and Caines, 1905.)
POTASSIUM SULFIDE K2S.
Fusion-point data for K2S + S are given by Thomas and Rule (1917).
POTASSIUM Antimony SULFIDE, see Potassium Sulfoantimonate, p. 500.
POTASSIUM TARTRATE (K2C4H4O6)2.H2O.
100 gms. H20 dissolve 138 gms. K2C4H4O6 at 16.6°, Sp. Gr. of sat. sol. = 1.49.
(Greenish and Smith, 1901.)
POTASSIUM (Bi) TARTRATE (Mono) KHC4H406, Cream of Tartar.
SOLUBILITY OF MONO POTASSIUM TARTRATE IN WATER.
(Afluard, 1865; Roelofsen, 1894; Blarez, 1891; at 20°, Magnanini, 1901; at 25°, Noyes and Clement, 1894.)
Gms. KHC4H4O6 per 100
t°. Gms. Solution. t°.
A
Gms. KHC4H406 per 100
Gms. Solution.
0
0.
30 (R.)
0.
32 (A.)
o,
35 (B.)
40
0.96
I.
3
1.29
IO
0.
37
0.
40
o
42
50
1.25
I,
8
i. 80
2O
0.
49
0.
53 (M.)
o,
60
60
2.
4
25
0.
58
0.
654 (N. and C.)
0.
74
80
. . .
4-
4
. . .
30
0.
69
0.
9 (A.)
0,
89
IOO
6.
3
SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS ALCOHOL AT 25°.
(Seidell, 1910.)
Wt. %
C2H5OH
in Solvent
du,oi
Sat. Sol.
Gms. KHC4H4O«
per loo Gms.
Sat. Sol.
Wt. %
C2H8OH
in Solvent.
<*25 Of
Sat. Sol.
Gms. KHC4H4O«
per loo Gms.
Sat. Sol.
0
I.OO2
0.649
50
0.912
0.064
IO
0.985
0.358
00
0.890
0.043
20
0.970
0.2IO
80
0.842
0.023
30
0-953
O.I3I
92.3
0.807
O.OI4
40
0-933
0.087
IOO
0.789
O.OIO
565
POTASSIUM BiTARTRATE
SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS ALCOHOL AT 18°.
(Paul, 1917.)
Cms. C2H5OH per 100 cc. solvent o 5
Gms. KHC4H4O6 per liter sat. sol. 4 . 903 3 . 58
2.94
10
2-57
Approximate determinations at other temperatures are given by Roelofsen
(1894) and by Wenger (1892).
SOLUBILITY OF MONO POTASSIUM TARTRATE (KHC4H4O6) IN NORMAL
SOLUTIONS OF ACIDS AT 20°.
(Ostwald; Huecke, 1884.)
Purified tartrate was added in excess to normal solutions of the acids, and, after
shaking, clear I cc. portions of each solution were withdrawn and titrated with
approximately o.i n Ba(OH)2 solution; I cc. normal acid requiring 10.63 cc» of
the Ba(OH)2 solution.
Acid.
Gms.
Acid
cc. N/io
Ba(OH)2
Gms.
KHC4H4O<
1 Acid
Gms. cc. N/io Gms
Acid Ba(OH)2 KHC4H4O6
per 100 cc. pei
Solvent. Sol
• i cc.
ution.
per loo cc.
Solution.
per 100 cc.
Solvent.
per i cc. per ico cc
Solution. Solution"
HNO3
6.
31
5
77*
10.
21
C2H5S03H
II. O
5
.01*
8.87
HC1
3-
65
5-
32
9-
42
HO.(CH2)2SO3H
12. 6l
5
•33
9-43
HBr
8.
IO
5-
38
9-
75
C6H5S03H
15.81
5
•25
9.29
HI
12.
80
5-
43
9-
61
HCOOH
4.60
0
•45
0.80
H2S04
4-
90
3-
97
7-
°3
CH3COOH
6.00
0
.27
0.48
HCH3SO4
ii.
21
5-
58
12.
44
CH2C1COOH
9-45
I,
.01
1.79
HC2H5S04
12.
61
9-
58
C2H5COOH
7.40
0
.24
0.42
HC3H7S04
14.
OI
5.
21
9-
22
C3H7COOH
8.81
0
•23
0.41
* The figures in this column show the amount of the Ba(OH>2 solution in excess of that which would
have been required by the normal acid solution alone in each case, viz., 10.63 cc. They, therefore, corre-
epond to the amount of KHC^Oo dissolved in i cc. of each saturated solution, and when multiplied
by i-77give the grams of KHC4H4Oe per 100 cc. solution.
SOLUBILITY OF MONO POTASSIUM TARTRATE (KHC4H4O6) IN AQUEOUS
SOLUTIONS OF ELECTROLYTES AT 25°.
(Noyes and Clement, 1894; Magnanini, 1901.)
Electro-
Gm. Equiv. per
Liter.
Gms. per
Liter.
Electro-
Gm. Equiv. per
Liter.
Gms. per
Liter.
lyte.
KC1
Electro- KHC4
lyte. H4O6.
0.025 0.0254
Electro-
lyte.
1.86
KHC4
HA
4.788
lyte.
CHsCOOK
Electro-
lyte.
0.05
KHC4*
HA.
0.0410
Electro-
lyte.
4.91
KHC4"
HA.
7.718
"
0.05
0.0196
3
•73
3-680
"
O. IO
o . 0504
9.82
9.486
u
O. IO
0.0133
7
.46
2.509
"
o. 20
0.0634
19.63
II.
930
11
O.2O
0.0087
14
.92
1.636
KHS04(2o°)
O.OI
0.0375
1-36
7-
06
KC103
0.025
0.0256
3
.06
4.821
"
O.O2
0.0500
2.72
9-
AI
u
0.05
0.0197
6
•13
3.716
"
O. IO
0.1597
13.62
30.
06
"
O. IO
0.0138
12
.26
2.601
KHC2O4* (20°)
O.OI
o . 0369
1.28
6.
94
"
O.2O
0.0097
24
• 52
1.728
a
0.02
o . 0424
2.56
7-
98
KBr
0.05
0.0192
5
•95
3.699
u
0.10
O.II32
12.82
21.
30
"
0.10
0.0134
ii
.91
2.517
HC1
0.013
0.0367
0-45
6.
90
"
o. 20
0.0087
23
.82
1.629
"
O.O25
0.0428
0.91
8.
06
KI
0.05
0.0196
8
•30
3.687
"
O.O5O
o . 0589
1.82
ii.
09
M
O. 10
0.0132
16
.61
2.492
Nad
0.05
0.0376
2.92
7-
08
u
o. 20
0.0086
33
.22
1.619
tt
O.IO
0.0397
5.85
7-
48
KNO3
0.05
0.0195
5-06
3.676
11
o. 20
0.0428
11.70
8.
05
u
O. IO
0.0136
IO
. 12
2.551
NaC103
0.05
0.0382
5-32
7-
18
"
o. 20
0.0090
20
.24
1.696
M
O.IO
o . 0405
10.65
7-
63
K2SO4
0.05
0.0208
4
.36
3.921
"
O.2O
0.0446
21.30
8.
40
"
0.10
0.0147
8
.72
2.769
M
0.20
O.OIOO
17
•44
1.888
* = acid potassium oxalate.
POTASSIUM TARTRATE 566
POTASSIUM Sodium TARTRATE. KNa.C4H4O6.4H2O. (Rochelle or Seig-
nette Salt.)
loo gms. sat. aq. solution contain 36.66 gms. KNaC4H4O6 at 9.7° and 47.97 gms.
at 29.5°. (van't Hoff and Goldschmidt, 1895.)
loo gms. H2O dissolve 53.53 gms. KNaC4H4O6 at 15°, Sp. Or. of sol. = 1.2713.
(Greenish & Smith, 1901.)
SOLUBILITY OF MIXTURES OF POTASSIUM TARTRATE AND OF SODIUM
TARTRATE IN WATER AT SEVERAL TEMPERATURES.
(van Leeuwen, 1897.)
AB Gms. per 100 Gms. Sat. Sol. Gms. per roo Gms. Sat. Sol.
* • '-K rwn '*r rwr> ' Solld Phase' * ' ' y r H n - - — ' Solld Phase*
K2C4H4U6. J\a2L4Jl4Us. Js.2^4Al4U6.
l8 19.2 16.5 KNaCiHiQs^HsiO 26.6 56 4.2 KNaC4H406.4H2O+K2T
38 26.6 22.8 " 48.3 51.6 13.2
20.9 ii. 8 28 " +Na*T 59-7 44-5 25.3
38 25.8 24.7 " " 80 39.7 34.7
50 36.7 23.9 "
K2T = K2C4H4O6.£H2O. Na2T = Na2C4H4O6.2H2O.
SOLUBILITY OF SEVERAL POTASSIUM SALTS OF TARTARIC ACIDS IN WATER AT 20°.
(Schlossberg, 1900.)
Salt. Formula. Q^^sS°
Potassium Sodium Salt of Racemic Acid KNa(C4H4O6).3H20 62.84
Potassium Sodium Salt of d Tartaric Acid KNa(C4H4O6).4H2O 63 . 50
Potassium Neutral Inactive Pyrotartrate K^CsHeOe.H^O 56.33
Potassium Neutral Dextropyrotartrate K^CsHeOe 57-62
•
SOLUBILITY OF POTASSIUM SODIUM TARTRATE IN AQ. ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1910.)
Wt. % , . Gms. Wt. % . . Gms.
QH6OH s^'c*, KNaC4HA.4H80 C2H5OH J*« 2* KNaC4H4O6.4H2O
in Solvent. bat" SoL per 100 Gms. Solvent in Solvent. bat' SoL per 100 Gms. Sat. Sol.
o 1.310 53.33 50 0.908 2.40
10 . 1.216 41.60 60 0.878 0.90
20 1.124 26.20 70 0-857 °-3°
30 1.034 13.80 80 0.840 0.06
40 0.961 6 100 0.789 trace
POTASSIUM DihydroxvTARTRATES K2C4H4O8.H2O and KHC4H4O8.H2O.
100 gms. H2O dissolve 2.66 gms. K^I^Os.HoO at o°. (Fenton, jSgS.)
100 gms. H2O dissolve 2.70 gms. KHC4H4O8.H2O at o°.
F.-pt. data for mixtures of d and / dimethyl ester of potassium bitartrate and
for mixtures of d and / diacetyl dimethylester of potassium bitartrate are given by
Adriani (1900).
POTASSIUM TELLURATE K2TeO4.
100 gms. H2O dissolve 8.82 gms. K2TeO4 at o°, 27.53 gms. at 20° and 50.42 gms.
at 30 . (Rosenheim and Weinheber, 1910-11.)
POTASSIUM THIOCYANATE KSCN.
SOLUBILITY IN WATER.
SStSSXL SolidPhase' Auttefty.
- 6.5
16.7
Ice (Rudorff, 1872.)
- 9-55
23.1
« «
—31.2 Eutec.
50.25
" +KSCN (Wassilijew, 1910.)
0
63-9
KSCN
20
68.5
" (Rudorff, 1869.)
25
70.5
" (Foote, 1903.)
567
POTASSIUM THIOCYANATE
SOLUBILITY OF MIXTURES OF POTASSIUM THIOCYANATE AND SILVER
THIOCYANATE IN WATER AT 25°.
(Foote, 1903.)
Solid
Phase.
KSCN
KSCN 4- zKSCN.AgSCN
Double Salt.
2KSCN.AgSCN =
53- 92% KSCN
2KSCN.AgSCN+
KSCNAgSCN
Double Salt.
KSCN .AgSCN =
36.9% KSCN
KSCN AgSCN + AgSCN
Gms. per
TOO Gms. Solution.
Mols. per
ioo Mols. H^O.
KSCN.
AgSCN.
KSCN.
AgSCN."
70-53
44.36
66-55
9-32
51 .13
4.19
64.47
10.62
47-98
4-60]
61 .25
II .76
42.07
4-7*1
.58.34
*3-55
38.47
5-23 1
53-21
17 .53
33-71
6.5oJ
50.68
20.43
32.52
7-67
49-43
32-51
20.32
18.34
30.29
12 .26
7.28^1
4-05 f
24.68
16.41
7-77
J
23.86
16.07
7-36
2.90
SOLUBILITY OF POTASSIUM THIOCYANATE IN ACETONE, AMYL ALCOHOL, ETC.
(von Laszcynski, 1894.)
In Acetone. In Amyl Alcohol. In Ethyl Acetate. In Pyridine.
Gms. KSCN per Gms. KSCN per Gms. KSCN per Gms. KSCN per
t°. 100 Gms. t°. 100 Gms. t°. 100 Gms. t°. 100 Gms.
(CH3)2CO.
CsHnOH.
CH3COOC2H6
CsHfiN.
22
20-75
13
0.18
o
0.44
0
6-75
58
20-40
65
i-34
14
0.40
20
6.15
100
2.14
79
O.2O
58
4-97
133-5
3-i5
97
3-88
"5
3.21
SOLUBILITY OF POTASSIUM THIOCYANATE IN PYRIDINE, DETERMINED BY
THE SYNTHETIC METHOD.
(Wagner and Zerner, 1911.)
-42
-42.1
-42.4
-42.8
Gms. KSCN
per loo Gms.
Mixture.
O
0-5
i-33
2.4
Solid
Phase.
Gms. KSCN
per loo Gms.
Mixture.
-43.3Eutec. 3.1
about +10 2.2
+KSCN
KSCN
70-71
II6-II7
172.7
173. 8m. pt.
Solid
Phase.
KSCN
1.23
0.89
at this temperature two liquid
layers appear and do not be-
come homogeneous up to 200°.
100 KSCN
ioo gms. anhydrous acetonitrile dissolve 11.31 gms. KSCN at 18°.
(Naumann and Schier, 1914.)
Fusion-point data for mixtures of KSCN + NaSCN and KSCN + RbSCN
are given by Wrzesnewsky (1912).
POTASSIUM THIOSULFATE
568
POTASSIUM THIOSULFATE
SOLUBILITY IN WATER.
Solid Phase.
(Jo, 1911,1912.)
O
Gms. K^Os
per ioo Gms.
H20.
96.1
17
I50-5
20
25
155-4
165
30
175-7
35
2O2.4
40
45
204.7
208.6
50
215.2
55
227.7
3K2S2O3.sH2O
t°.
Gms. K2Sj03
per ioo Gms.
H20.
56.1
234-5
60
238.3
65
245-8
70
255-2
75
268
78.3
292
80
293.1
85
298.5
90
312
Solid Phase.
2S2O3.H2O
3K2SA.H20
POTASSIUM Sodium THIOSULFATE KNaS2O3.2H2O.
100 gms. H2O dissolve 213.7 Sms- KNaS2O3.2H2O (a) at 15°.
100 gms. H2O dissolve 205.3 gms. KNaS2O3.2H2O (6) at 15°.
(Schwicker, 1889.)
POTASSIUT3 FluoTITANATE K2TiF6.H2O.
SOLUBILITY IN WATER. (Marignac, 1866.)
t°. o°. 3°. 6°. 10°. 14°. 20°.
Gms. K2TiF6 per ioo gms. H20 0.55 0.67 0.77 0.91 1.04 1.28
POTASSIUM VANADATE K3V5O14.5H2O.
ioo gms. H2O dissolve 19.2 gms. at 17.5°. (Radan. 1889.)
POTASSIUM ZINC VANADATE KZnV6O14.8H2O.
ioo gms. H2O dissolve 0.41 gm. of the salt (Radan).
PRASEODYMIUM CHLORIDE PrCl3.
SOLUBILITY IN WATER, AQ. HYDROCHLORIC ACID AND IN PYRIDINE.
(Matignon, 1906, 1909.)
Solvent. t°. Sp. Gr. Sat. Sol. Gms. per ioo Gms. Sat. Sol.
Water 13 1.687 5o.96PrCl3
Aq.HCl 13 1.574 4i.o5PrCld-7.25HCl
Pyridine room temp. ... 2.1 PrCls
PRASEODYMIUM GLYCOLATE Pr2(C2H3O3)3.
One liter water dissolves 3.578 gms. Pr2(C2H3O3)3 at 20°. Qantsch & Grunkraut, '12-13.)
PRASEODYMIUM MOLYBDATE Pr2(MoO4)8.
One liter water dissolves 0.0152 gm. Pr2(MoO4)3 at 23° and 0.0143 gms. at 75°.
(Hitchcock, 1895.
PRASEODYMIUM Double NITRATES
SOLUBILITY AT 16° IN CONC. HNO3 OF
Salt.
^=1.325. (Jantsch, 1912.)
Gms. Hydrated
Formula. Salt per ioo cc.
Sat. Solution.
Praseodymium Magnesium Nitrate
Nickel
Cobalt
Zinc
Manganese "
Ni3
Co3
Zn3
Mn3
7.70
9.28
12.99
14.69
23.40
569 PRASEODYMIUM OXALATE
PRASEODYMIUM OXALATE Pr2(C2O4)8.ioH2O.
One liter H2O dissolves 0.00074 Sm- Pr2(C2O4)3 at 25°. (Rimbach and Schubert, 1909.)
ioo gms. aq. 19.4% HNO3 (d = 1.116) dissolve 1.16 gms. Pr2(C2O4)3 at 15°.
(v. Scheele, 1899.)
ioo gms. aq. 10.2% HNO3 (d = 1.063) dissolve 0.50 gm. Pr2(C2O4)3 at 15°.
Cv. Scheele, 1899.)
PRASEODYMIUM Dimethyl PHOSPHATE Pr2[(CH3)2PO4]6.
IOO gms. H2O dissolve 64.1 gm. Pr2[(CH3)2PO4]e at 25°. (Morgan and James, 1914.)
PRASEODYMIUM SULFATE Pr2(SO4)3.
SOLUBILITY IN WATER. (Muthmann and Rolig, 1898.)
Solid
Phase.
Pr2(S04)3.8H20
Pr2(S04)3.8H20 +
Pr2(S04)3.5H20
PRASEODYMIUM SULFONATES
SOLUBILITY IN WATER.
Gms. Pr2(SO4)3
t " per ioo Gms.
Solid + o
Phase. '
Gms. Pr2(SO4)s
per loo^Gms.
Solution.
Water.
Solution.
Water.
0
I6.S
19.8
Pr2(S04)3.8H20 75
4-0
4-2
18
12-3
I4.I
8S
J-5
i-55
35
9-4
10-4
"
55
6,6
7-1
95
I.O
1. 01
Praseodymium Salt of:
Bromonitrobenzene Sulfonic Acid
Benzene Sulfonic Acid
m Nitrobenzene Sulfonic Acid
m Chlorobenzene Sulfonic Acid
Chloronitrobenzene Sulfonic Acid
a Naphthalene Sulfonic Acid
1.5 Nitronaphthalene Sulfonic Acid
1.6
1.7
Formula.
Pr(C6H3.Br.N02.S03)i,4,2)s.-
8H2O
Pr(C6H6S03)3.9H20
Pr[C6H4(N02)S03]3.6H2O
PrICeH4Cl.S03j3.9H20
Pr (C6H3.SO3.NO2.Cl,i ,3,6)3.-
i4H2O
Pr[C10H7S03]3.6H20
,. 6B,O
. 9H20
.nH2O
Gms. Anhy-
drous Salt
per ioo Gms.
H20.
6 . 08 (Katz& James, '13.)
Authority.
55-6
33-9
12.6
25-9
6.1
0.47
0.18
(Holmberg, 1907.)
PRASEODYMIUM TUNGSTATE Pr2(WO4)3.
One liter water dissolves 0.0438 gm. Pr2(WO4)3 at 75°.
PROPIONIC ACID C2H5COOH.
(Hitchcock, 1895.)
SOLUBILITY IN WATER, DETERMINED BY THE FREEZING-POINT METHOD.
(Faucon, 1910.)
t°of
Solidif.
-17.2
— 21
t° of Gms. C2H5COOH « ,. , p..
Solidif. per ioo Gms. Sol. Sohd Phase'
-1.33 4.98 Ice
—2.60 10. ii
- 3.76
— 6. 10
- 7.70
15
25
35.
28
— 9.20
-10.80
— 14.20
45
55
65
.20
.88
Gms. C2H5COOH
per ioo Gms. Sol.
73.48 Ice
Sl-75
86.85
87.65
89.12
92.40
97.22
IOO
Solid Phase.
+C2HJCOOH
QHsCOOH
— 29.10
— 29.40
-28.30
— 26 . 90
- 23 . 90
— 19.30
Additional data for this system are given by Tsakalatos (1914), Herz (1917) and
Ballo (1910). The last-named investigator also determined the composition of
the solid phases and explains the abnormal freezing-point lowering on the basis of
production of mix-crystals.
The ratio of distribution of propionic acid between water and benzene was
found by King and Narracott (1909) to be 1:0.129 at room temperature.
PROPIONIC ACID 570
DISTRIBUTION OF PROPIONIC ACID BETWEEN ETHER AND AQUEOUS SALT
SOLUTIONS AT l8°. (de Kolossovsky, 191 1.)
Aq. Salt Solution (2 Mols. per Liter). QHsCOOH per 100 cc. of:
Salt.
Gms. Salt per 100 cc.
Aq. Layer (q).
Ether Layer (q1).
q''
Water alone
I.I7O
2.305
0.50
NaCl
11.69
0.762
2-543
0.30
MgCl2
19.05
0.567
3.I35
0.18
KNO3
20.22
0.972
2.298
0.42
KC3H40
1 22.43
L324
2.406
o-55
P lodoPROPIONIC ACID CH2I.CH2.COOH.
One liter sat. solution in water contains 80 gms. CH2I CH2COOH at 25°.
(Sidgwick, 1910.)
One liter sat. solution in i n aq. sodium ft iodopropionate contains 126 gms. at
25°. (Sidgwick, 1910.)
0 PhenylPROPIONIC ACID (Hydrocinnamic Acid) CH2(C6H6).CH2COOH.
SOLUBILITY IN WATER AND IN AQ. NORMAL SODIUM ft PHENYLPROPIONATE.
(Sidgwick, 1910.)
Gms. CH2(C6HS)CH2COOH per Liter Solution at:
Solvent. , * >
11°. 25°.
Water 4.80 7.5
i n aq. CH2(C6H6)CH2.COONa 7 . 65 172.5 (liquid layers formed)
SOLUBILITY OF ft PHENYLPROPIONIC ACID IN WATER AND IN ALCOHOLS.
(Timofeiew, 1894.)
Gms. CH2(C,H6)- Gms. CH2(C,H5)
Almhnl t° CHjCOOH per Almhnl t° CH2COOH per
ioo Gms. Sat. 100 Gms. Sat.
Solution. Solution.
Water 19 0.7 Ethyl Alcohol +19.6 77.2
Methyl Alcohol -18.5 55.8 " " 20 78.8
-16 57.6 Propyl Alcohol -18.5 35
" " o 66.9 " " -16 39
+ 19.6 82.8 " " +19.6 73.4
20 83.8 " " 20 73.9
Ethyl " —18.5 46 Isobutyl Alcohol 19.6 67.3
-16 48
SOLUBILITY OF ft PHENYLPROPIONIC ACID IN SEVERAL SOLVENTS.
(Herz and Rathmann, 1913.)
CH2(C«H5) CH2.COOH CH2(C6H6) CH2COOH
Solvent. Per Liter. Solyent per Liter.
Mols. Gms. Mols. Gms.
Chloroform 5 . 444 817.2 Tetrachloro Ethylene 4.725 709 . 2
Carbon Tetrachloride 4.604 691.1 Tetrachloro Ethane 5.430 815.1
Trichloro Ethylene 5.140 771.6 Pentachloro Ethane 5.019 753.4
P Phenyl DibromoPROPIONIC ACID C2H2Br2(C6H6)COOH.
ioo cc. sat. sol. in carbon tetrachloride contain o. 124 gm. acid at 26°. (De Jong, 1909.)
ioo cc. sat. sol. in petroleum ether contain 0.072 gm. acid at 26°.
PhenylPROPIOLIC ACID C6H6C : C.COOH.
SOLUBILITY IN SEVERAL SOLVENTS. (Herz and Rathmann, 1913.)
C6H6C:C COOH C6HBC:C.COOH
Solvent. per Liter. Solvent. per Liter.
Mols. Gms. Mols. Gms.
Chloroform 0.789115.30 Tetrachloro Ethylene 0.324 47.34
Carbon Tetrachloride 0.227 33.16 Tetrachloro Ethane 0.718104.90
Trichloro Ethylene 0.382 55.82 Pentachloro Ethane 0.410 59.91
PROPIONIC ALDEHYDE C2H5COH.
ioo gms. H2O dissolve 16 gms. aldehyde at 20°. (Vaubel, 1899.)
571 PROPIONITRILE
PROPIONITRILE C2H5CN.
SOLUBILITY IN WATER.
Synthetic method used. See Note, p. 16. (Rothmund, 1898.)
Wt. per cent C2H5CN in: Wt. per cent C2H5CN in:
*° ' Aq C2H6CN *"• A^ C2HSCN
Layer. Layer. Layer. Layer.
40 10.7 92.1 95 19.6 78.0
50 ii. 6 90.5 ioo 22.4 75.5
60 12.7 88.5 105 26.0 72.1
70 13.2 86.1 no 32.0 66.5
80 14-9 83.4 113 .1 (crit. temp.) 48.3
90 17.6 80.2
PROPYL ACETATE, Butyrate and Propionate.
SOLUBILITY OF EACH IN AQUEOUS ALCOHOL MIXTURES.
(Bancroft — Phys. Rev. 3, 205, '95, calc. from Pfeiffer.)
cc. Alco-
hol in
P. Ace-
P. Butyr
P. Propio-
cc. Alco-
hol in
P. Ace-
P. Buty-
P. Propio-
Mixture.
tate.
rate.
nate.
Mixture.
tate.
rate.
nate.
3
4-5°
I.I9
I.58
21
58-7I
19.68
27.83
6
10.48
3-55
4.70
24
00
23.72
33-75
9
17.80
6.13
8-35
30
32.10
47-15
12
26.00
9-o5
12.54
36
41-55
63.18
15
35-63
12.31
17-15
42
51 .60
83-05
18
47-50
15.90
22.27
48
62 .40
107.46
54
73 85
* cc. H2O added to cause the separation of a second phase in mixtures of the given amounts of alcohol
and 3 cc. portions of propyl acetate, butyrate and propionate
SOLUBILITY OF PROPYL ACETATE, FORMATE, AND PROPIONATE IN WATER.
100 cc. H2O dissolve 1.7 gms. propyl acetate at 22°. (Traube, 1884.)
100 cc. H2O dissolve 2.1 gms. propyl formate at 22°.
100 cc. H2O dissolve 0.6 cc. propyl propionate at 25°. (Bancroft, 1895.)
PROPYL ALCOHOL C3H7OH.
Freezing-point data (solubilities, see footnote, p. i) for mixtures of propyl
alcohol and water are given by Pickering (1893). Results for mixtures of iso-
propyl alcohol and water are given by Dreyer (1913).
100 gms. sat. solution of propyl alcohol in liquid carbon dioxide contain 36.5
gms. C3H7OH at —24° and 57.5 gms. at —30°. (Buchner, 1905-06.)
MISCIBILITY OF PROPYL ALCOHOL WITH MIXTURES OF CHLOROFORM AND
WATER AT o°.
(Bonner, 1910.)
See Notes, pp. 14 and 287.
Composition of Homogeneous Mixtures. Composition of Homogeneous Mixtures.
Gms. CHC13.
Gms. H2O.
Gms.
C3H7OH.
Sp. Gr. of
Mixture.
Gms. CHC13.
Gms. H2O.
Gms.
C3H7OH.
Sp. Gr. of
Mixture.
0.977
O.O23
0.304
1.28
0.500
0.50
1-34
0.97
0.926
0.074
0.631
I-I3
0-394
0.6o6
1.32
0.98
0.90
0.10
0.76
I .11
0.293
0.707
1-235
0.96
0.80
0.20
1. 06
1.04
0.194
0.8o6
0.996
°-95
0.70
0.30
I .20
1. 01
0.097
0.903
0.672
0.97
0.60
0.40
1.30
0.98
0.030
0.97
0-39
0.97
PROPYL ALCOHOL
572
MISCIBILITY OF PROPYL ALCOHOL AT o° WITH MIXTURES OF:
Carbon Tetrachloride and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Ethyl Bromide and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Cms. CC14.
Cms. H2O.
Cms.
C3H7OH.
Sp. Gr. of
Mixture.
Cms.
C2HBBr.
Cms. H2O.
Cms.
C3H7OH.
Sp. Gr. of
Mixture.
o-975
0.025
0.317
I-3I
0.941
0.039
0.367
I. 21
0.931
0.069
0.536
I.I7
0.912
0.088
0.615
I. II
0.90
O.IO
0.65
I.I4
0.90
O. IO
0.64
I.IO
0.80
0.2O
0.949
1.07
0.80
0.2O
0.85
1-05
0.70
0.30
I. 12
1 .02
o. 70
0.30
I
I. O2
0.60
0.40
I. 20
0.99
0.6o
0.40
1.09
I
0.499
0.501
1-234
0.98
0.491
0.509
I.I24
0.98
0.40
O.60
I-I95
0-97
0.40
0.60
I. 10
0.97
0.30
0.70
I.I3
0.96
,0.30
0.70
0.90
0.96
*0.25
0-75
I. 06
0.20
0.80
0.81
0.96
0.194
0.806
0.912
0.96
o. 14
0.86
0.671
0.96
O. IOO
0.90
0.68
0.96
O.IO
0.90
0.56
0-97
0.013
0.987
0-354
0.96
*0.023
0.977
0.227
0.99
See Notes, pp. 14 and 287.
MISCIBILITY OF PROPYL ALCOHOL AT o° WITH MIXTURES OF:
Bromobenzene and Water. (Bonner, 1910.) Bromotoluene and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures. Composition of Homogeneous Mixtures.
Gms. C6H6Br.
Gms. H2O.
Gms.
C3H7OH.
Sp. Gr. of
Mixture.
Gms.
C6H4CH3Br.
Gms. H2O.
Gms.
C3H7OH.
Sp. Gr. of
Mixture.
0.983
O.OI7
0.186
1.29
0.968
0.032
0.252
1.23
0.909
0.091
0.56
I. II
0.90
O. IO
0.52
I. II
0.90
O.IO
0.58
I. II
0.80
0.20
0.78
1.03
0.80
0.20
0.87
1.05
0.70
0.30
0.96
I. 01
0.70
0.30
1.05
1 .02
0.6o
0.4O
1.07
0.99
0.60
O.40
I-I5
I
0.50
0.50
I-I3
0.97
0.50
0.50
I.I9
0.97
0.40
0.60
I-I3
0.96
0.40
0.60
I.I9
0-97
0.30
O.7O
1.03
0-95
0.30
0.70
1.09
0-95
*0.25
0-75
0.97
O. 20
0.80
0-93
0-95
0. 20
0.80
0.90
0.94
O. IO
0.90
0.71
0.96
O.IO
0.90
0.72
0-95
0.021
0.979
o-457
0.98
0.013
0.987
0.424
0.96
See Notes, pp. 14 and 287.
DISTRIBUTION OF PROPYL ALCOHOL BETWEEN WATER AND COTTON-SEED
OIL AT 25°.
(Wroth and Reid, 1916.)
Oil Layer.
1.447
1-475
1-503
H2O Layer.
8. 112
8.897
9.809
5-60
6. 10
6-53
Oil Layer.
I.5l6
I-576
1.694
H2O Layer.
10.07
10.49
10.41
6.64
6.65
6. 14
Data for systems composed of normal propyl alcohol, water and various in-
organic salts are given by Timmermans, 1907.
PROPYLAMINE CH3.CH2.CH2.NH2.
The solubility of propylamine in water at 60°, determined by an aspiration
method using an indifferent gas, is 191 when expressed in terms of the Bunsen
absorption coefficient 0 (see p. 227) and /6o = 233 when expressed in terms of the
Ostwald solubility expression. (Doyer, 1890.)
573
PROPYL AMINES
Freezing-point data for mixtures of propylamine and water, isopropylamine
and water and for dipropylamine and water are given by Pickering (1893).
DISTRIBUTION OF PROPYLAMINES BETWEEN WATER AND TOLUENE.
(Moore and Winmill, 1912.)
Results at 18°.
Amine.
Gm. Equiv.
Amine per
Liter of Aq.
Layer.
Propylamine o . 0973
" 0.0928
Dipropylamine o . 0764
0.0794
Tripropylamine 0.0003
Partition
Coef.
434
439
0.1185
0.1188
0.003
Partition
Coef.
Results at 25°.
Gm. Equiv.
Amine per
Liter of Aq.
Layer.
0.03837
o . 04300
O.O722
0.0681
4.470
4.470
0.0769
0.0771
Results at 32.35°.
Gm. Equiv.
Amine per
Liter of Aq.
Layer.
o . 0602
0.0578
O. OIl68
O.OII99
Partition
Coef.
3-3I7
0.05802
0-05795
PROPYLAMINE HYDROCHLORIDE a NH2(C3H7).HC1.
100 gms. H2O dissolve 278.2 gms. NH2(C3H7).HC1 at 25°. (Peddle and Turner, 1913.)
100 gms. CHC13 dissolve 5.26 gms. NHi(C3H7).HCl at 25°. (Peddle and Turner, 1913.)
DiPROPYL AMINE HYDROCHLORIDE NH(C3H7)2.HC1.
IOO gms. H2O dissolve 165.3 Sms- NH(C3H7)2.HC1 at 25°. (Peddle'and Turner, 1913.)
100 gms. CHC13 dissolve 47.24 gms. NH(C3H7)2.HC1 at 25°. (Peddle and Turner, 1913.)
PROPYL CHLORIDE, Bromide, etc.
SOLUBILITY IN WATER.
(Rex, 1906.)
Propyl Compound.
CH3CH2CH2C1 (normal)
CH3CH2CH2Br "
CH3CH2CH2I
(CH3)2CHC1 (iso)
(CH3)2CHBr «
(CH3)2CHI «
Grams P. Compound per 100 Gms. HjO at:
0°.
10°.
20°.
30°.
0.376
0.323
0.272
0.277
0.298
0.263
0.245
0.247
0.114
0.103
O.IO7
0.103
0.440
0.363
0.305
0.304
0.418
o-365
0.318
0.3l8
0.167
0.143
O.I4O
0.134
PROPYLENE C8H6.
SOLUBILITY IN WATER.
(Than, 1862.)
t". ft. q.
o 0.4465 0.0834
5 0.3493 0.06504
10 0.2796 0.0519
15 0.2366 0.0437
20 0.2205 0.0405
For values of /3 and q, see Ethane, p. 285.
PYRENE C16H10
SOLUBILITY IN TOLUENE AND IN ABSOLUTE ALCOHOL.
100 gms. toluene dissolve 16.54 Sms- pyrene at 18°.
100 gms. absolute alcohol dissolve 1.37 gms. pyrene at 10° and 3.08 gms. at
b. pt.
PYRIDINE
574
PYRIDINE CH < (CH.CH)2 > N.
SOLUBILITY IN WATER, DETERMINED BY THE FREEZING-POINT METHOD.
(Average curve from results of Pickering (1893) and Baud (1909.)
t'.of
Solidi-
fication.
Gms.
C5H6N per
100 Gms.
Mixture.
Solid
Phase.
0
0
Ice
— I
7-5
"
— 2
i7
"
-3
28
u
-4
37-5
"
-5
43-5
"
-6
48
«
Q
54
"
Gms.
C6H6Nper Solid
J.G nt
Gms.
C*H*N Per
Solid
phase-
— 10
— 12.
-15
— 20
-25
-30
-40
-50
58
62
64
68
7i
73
78
81
5 Ice
-60
-65 Eutec.
-60
-55
-50
-45
-40
84
85
87
89
92
95
97
Ice
+CtHjN
— 38 m. pt. 100
Timmermans (1912) is reported to have made determinations on the above
systems but the original paper could not be located.
Baud also gives data for the densities of pyridine + water mixtures.
DISTRIBUTION OF PYRIDINE BETWEEN WATER AND BENZENE.
At Room Temperature.
(v. Georgievics, 1915.)
Gms. CSH5N per
At 25°.
(Hantzsch and Sebaldt, 1899.)
Mols. C8H5N per Liter.
25 cc. H2O Layer.
0.0617
0.0958
0.1549
0.2432
0.3297
0.723
1. 147
75 cc. CeH6 Layer.
0.4733
0.7631
1.2249
2.0096
2.6553
5-4I59
9.878
Aq. Layer.
C6H6 Layer.
rs.ai.io.
O.OOI48
0.00436
0-339
0.00076
0.00226
0-339
0.00038
O.OOIIO
0-345
O.OOO2O8
O.OOO546
0.381
O.OOOII2
0.000274
0.413
(at
5.5°) 0.000456
O.OOO928
0.491
(at
50°) O.OOO3I4
O.OOIO88
0.289
DISTRIBUTION OF PYRIDINE BETWEEN WATER AND TOLUENE.
(Hantzsch and Vagt, 1901.)
At 25°.
er Liter.
Ratio.
0.458
0.466
0.481
0.496
0.551
0.629
0.647
0.696
Data for systems composed of py
given by Timmermans, 1907.
Methyl PYRIDINES
Data for the reciprocal solubility of 3 methyl pyridine { = 0 picoline) and
water, 2.6 dimethyl pyridine (= 2.6 lutidine) and water, methyl pyridine (=7
picoline) zinc chloride and water, methyl pyridine zinc chloride and each of the
following alcohols; methyl, ethyl, propyl, isobutyl, isoamyl, cetyl and methyl
hexylcarbinol, determined by the synthetic method (see Note, p. 16), are given by
'Flaschner (1909). See also p. 262, for2.4.6trimethyl pyridine (collidine) and water.
Mols. C6HBN per Liter.
Aq. Layer.
C«H&CH3 Layer.
0.0517
0.026l
O.II29
0.0559
O.OI32
0.0067
0.0033
0.0275
0.0137
0.0066
O.OOI9
O.OO34
O.OOII
0.0017
0.0007
0.0010
At Various Temperatures.
Mols. C5H5N per Liter.
t° * Ratio
Aq. Layer. C6H5CH3 Layer.
0
0.0168
O.O2OI
0.840
10
0.0135
0.0215
0.627
20
O.OIII
0.0228
0.529
30
0.0108
0.0234
0.461
40
O.OIOI
0.0245
0.411
50
0.0096
0.0252
0.380
70
0.0085
0.0263
0-324
90
0.0082
0.0266
0.307
e, water and various inorga:
nic salts are
575
PYRIDINE
PYRIDINAMINO SUCCINIC ACIDS.
100 gms. H2O dissolve 1.67 gms. of the d compound, 1.64 gms of the / com-
pound and 1.68 gms. of the dl compound at 18°. (Lutz, 1910.)
PYROCATECHOL o C6H4(OH)2.
100 gms. H29 dissolve 45.1 gms. C6H4(OH)2 at 20°. (Vaubel, 1899.)
100 gms. pyridine dissolve an unlimited amount of CeH^OH^ at 20°. (Dehn, 1917.)
100 gms. aq. 50% pyridine dissolve 101 + gms. of CeH^OH^ at 20-25°. "
F.-pt. data for pyrocatechol + resorcinol are given by Jaeger (1907).
PYROGALLOL C6H3(OH)3 i, 2, 3.
SOLUBILITY IN WATER, ETC.
(U. S. P. VIII.)
ioo gms. water dissolve 62.5 gms. C6H3(OH)3 at 25°^.
100 gms. alcohol dissolve ioo gmi
ioo gms. ether dissolve 90.9 gms.
ioo gms. alcohol dissolve ioo gms. C6H3(OH)3 at 25°.
jms. CeHa(OH), at 25°.
Dimethyl PYRONE C7H8O2.
Freezing-point data for mixtures of dimethyl pyrone and each of the following
compounds: salicylic acid, 0, m, p and a toluic acids and trinitrotoluene are given
by Kendall (i9i4a). Results for mixtures of dimethyl pyrone and sulfuric acid
are given by Kendall and Carpenter (1914).
QUINHYDRONE
Data for the solubility and dissociation of quinhydrone in water at 25° are
given by Luther and Leubner (1912).
QUINIDINE C2oH24N202. ?H2O.
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent. t°.
Water 18-22
Water 25
Ethyl Alcohol (95%) 20
Ethyl Alcohol
Methyl Alcohol
Benzene
Benzene
Carbon Tetrachloride
Chloroform
Chloroform
Ether (d = 0.72)
Ether sat. with H2O
H2O sat. with Ether
Ethyl Acetate
Pet. Ether (b. pt. 59°-64°)
i vol. C2H5OH+4 vols. CHCU
i vol. C2H5OH+4 vols. C6H6
i vol. CH3OH+4 vols. CHCla
i vol. CH3OH+4 vols.
QUINIDINE SALTS
Gms.
Gms. Solvent.
O.O2O
I24 N2O2 per ioo.
cc. Solvent.
Authority.
25
25
25
1 8-2 2
2-45
1 8-2 2
°-SS7
18-22
IOO+
25
1 8-2 2
0.78
1 8-2 2
1.63
1 8-2 2
0.031
1 8-2 2
1.76
1 8-2 2
0.024
25
25
25
25
(Mullet, 1903.)
0.0145 (Schaefer, 1910.)
(Wherry & Yanovsky, 1918.)
(Schaefer, 1913.)
22
66
33-3
12.5
25
6.6
(Muller, 1903.)
(Schaefer, 1913.)
(Muller, 1903.)
(Schaefer, 1913.)
Quinidine Salt.
Q. Hydrobromide
Q. Hydrochloride
Q. Hydroiodide
Q. Salicylate 0.060
SOLUBILITY IN WATER AT 25°.
(Schaefer, 1910.)
Gms. Salt per
loo Gms. H2O.
0.526
1. 160
0.082
Quinidine Salt.
Q. Sulfate
Q. Tannate
Q. Tartrate
O. Bitartrate
Gms. Salt per
100 Gms. H2O.
1.05
0.0477
2.86
0.323
QUINIDINE SULFATE
576
SOLUBILITY OF QUINIDINE SULFATE IN SEVERAL SOLVENTS AT 25°.
(Schaefer, 1913.)
Solvent.
Ethyl Alcohol
Methyl Alcohol
Chloroform
Benzene
Cms. Q. Sulfate
per too cc.
Solvent.
5
40
Insol.
Solvent.
i vol. C2H6OH+4 vols. CHC13
i vol. C2H5OH+4 vols. C6H6
i vol. CH3OH+4 vols. CHCls
i vol. CHaOH+4 vols. CeH6
Cms. Q. Sulfate
per too cc.
Solvent.
33-3
8-33
33-3
20
QUININE C2oH24N2O2.3H2O.
Solvent.
Water
Ethyl Alcohol
Methyl Alcohol
Benzene
Aniline
Carbon Tetrachloride
Chloroform
«
Diethylamine
Ether
SOLUBILITY IN SEVERAL SOLVENTS.
sat. with H2O
H2O sat. with Ether
Ethyl Acetate
Petroleum Ether (b.
pt. 59°-64°)
Oil of Sesame
Glycerol
Piperidine
Pyridine
Aq. 50% Pyridine
7.65gms.H3BO3perioo room
cc. aq. 50% Glycerol temp.
i5.3gms.H3BO3perioo room
cc. aq. 50% Glycerol temp.
Anhydrous Quinine
A0 Gms. per 100.
Hydrated
oJU^oo Authority.
Gms. Solvent.
Gms.
Solvent.
CC.
Solvent.
18-22
0.051
0.05 74 (Muller, 1903.)
25
0.057
0.
033
0.065
(U. S. P.; Schaefer, 1910.)
80
0.123
0.129
(U. S. P.)
20
100
. .
.
(Wherry and Yanovsky, 1918.)
25
166.6
.
i6o\6
(U. S. P.)
25
. . .
1333
(Schaefer, 1913.)
2O
66.
6
.
•' .:•
25
o.
55
0.205
(Schaefer; Muller, 1903.)
2O
0-5
.
(Wherry and Yanovsky, 1918.)
1 8-2 2
.
(Muller, 1903.)
20
14-5
.
(Scholtz, 1912.)
20
0-54
.
0.204
(Gori, 1913; Muller, 1903.)
25
50-52.6
. .
.
62.5
(Schaefer, 1913; U. S. P.)
18-22
100 -f-
. .
.
loo +
(Muller, 1903.)
20
57
. .
.
(Scholtz, 1912.)
25
22.2
. .
.
76.9
(U. S. P.)
1 8-2 2
0.876
. .
.
1.62
(Miiller, 1903.)
1 8-2 2
2.8
»
5-62
"
1 8-2 2
0.085
0.067
"
1 8-2 2
24-7
. -
4-65
"
18-28
20
25
2O
20
20-25
0.021
0.633
IIQ
IOI
59-4
20
40
O.OIO
0.053
0.472
(Zalai, 1910.)
(U. S. P.; Ossendowski, 1907.)
(Scholtz, 1912.)
(Dehn, 1917.)
(Baroni and Barlinetto, 1911.)
SOLUBILITY OF QUININE IN BENZENE, DETERMINED BY THE SYNTHETIC
(SEALED TUBE) METHOD.
(van Iterson-Rotgans, 1914.)
*"' Qubint Solid Phase.
53-5 4-8r
63 6 . 09 Mixed phase,
91 30.01 probably a
I O2 43 • 4 colloid or sol-
104 .5 45 . 9 ution of high
109 51.8 viscosity.
130 75.46
* Eutec.
t".
Wt. %
Quinine.
Solid Phase.
5-4
0
QH,
5-3*
17
0.72 c
29
1.48
"
38.5
2-36
«
49
5.22
" unstable
±70
28.9
U «
t°.
<SSL£"" .«—
137
80 CajH^NA
142
83.04
146
85.26
152
87.44
158.5
91.4
166
95-02
174.7 loo
577
QUININE
SOLUBILITY OF QUININE IN AQUEOUS SOLUTIONS OF CAUSTIC ALKALIES.
(Doumer and Deraux, 1895.)
METHOD. — A one per cent solution of quinine sulfate, containing a very
small amount of HC1, was gradually added to 200 cc. portions of the caustic
alkali solutions of the various concentrations stated, and the point noted at which
a precipitate of the appearance corresponding to that of I cc. of milk in 100 cc.
of water, remained undissolved.
In Aq. Ammonia. In Aq. Sodium Hydroxide. In Aq. Pot. Hydroxide.
Gms. NH3 Gms. Anhydrous
Gms. NaOH
Gms. Anhydrous
Gms. KOH
Gms. Anhydrous
per 200 cc.
Solution.
Quinine
Dissolved.
per 200 cc.
Solution.
Quinine
Dissolved.
per 200 cc.
Solution.
Quinine
Dissolved.
0.52
0.084
0.007
0.092
0.612
0.088
0.65
0.084
O.OI2
0.091
I.5I2
0.082
4-59
0.096
0.740
0.090
3-456
0.068
13.08
0.122
2.l6o
0.079
10.944
0.039
18.88
0.144
3-188
0.056
44.704
0.006
25.19
0.174
6. 172
0.044
35-79
0.184
8-537
O.O2I
17.074
0.015
SOLUBILITY OF QUININE SALTS IN WATER.
(Regnault and Willejean, 1887.)
Salt.
Brom Hydrate (basic)
" (neutral)
Chlor Hydrate (basic)
Lactate (basic)
AO Gms. Salt per
' 100 Gms. H2O.
14
2.06
12
12.33
14
16
13-19
14-79
15
12
14.20
3-8o
14
4.14
15
4-25
15
37
10.03
16.18
Salt.
j-o Gms. Salt per
too Gms. H2O.
Salicylate (basic)
15 0.114
Sulfate "
14 0.139
« a
16 0.153
tt «
18 0.160
" (neutral)
15 8.50
« «
17 8.90
« «
18 9.62
Valerate (basic)
12-16 2.59
SOLUBILITY OF QUININE SALTS IN WATER AT 25°.
(Schaefer, 1910.)
Salt.
Gms. Salt per
100 Gms. H2O.
Acetate
2
Anisol
0.042
Arsenate
0.154
Benzoate
0.278
Bihydrobromide
20
Bihydrochloride
143 (133)
Bihydrochloride + Urea
100
Bisulfate
11.78
Chlorhydrosulfate
77 (So)
Chromate
0.032
Citrate
O. 121 (0.083)
Glycerophosphate, basic
o. 1178 (insol.)
Hydrobromide
2-33
Hydrochloride
4.76
Hydroferrocyanide
0.05
Hydroiodide
0.49
* Insol.
Salt.
Gms. Salt per
100 Gms. H2O
Hypophosphite
2.85
Lactate, basic
16.6
Nitrate
T-43
Oxalate
0.071
Phosphate
0.125
Picrate
0.029
Quinate
. 28.6
Salicylate
0.048
Sulfate
0.143
Bisulfoguiacolate
200
Sulfophenate
0.4
Urate
O.l82
Phenylsulfate
0.147
Tartrate
o. 105
Tannate
o.o5(*)
Valerate
1.25
It is pointed out that different values for the solubility may be obtained de-
pending on the method used for preparing the saturated solution.
Results in parentheses are by Squire and Caines (1905), and are for I5°-2O°
instead of 25°.
QUININE SALTS
578
SOLUBILITY OF QUININE SALTS IN SEVERAL SOLVENTS.
(Phelps and Palmer, 1917-)
Solubility, Parts per 100 Parts Solvent in:
Salt.
M. pt.
(uncorr.)
ecu. (
CHC13. Ethyl Acetate (Alcohol free) .
\lcoholfree). Cold. Hot.
Quinine racemic lactate 165 . 5
0.00715
28.6 0.286 3.33
d lactate
175
O.OIII
0.25
/
171
0.00476
O.2O
formate
IIO-II3
0.00625
... ... ...
acetate
124-126
0.05
... ... ...
propionate
IIO-III
0.238
... ... ...
butyrate
77-5
4
... ... ...
succinate
192
O.OOI
0.4
tartrate
202.5
0.0004
... ... 0.0333
malate
177-5
0.0008
0.5
citrate
i83-S
0.00167
0.0833
sulfate
214
0.0025
0.0333 0.00715 0.0133
Quintoxime lactate
O. II
... ... ...
Saturation was obtained by shaking at intervals by hand, during 72 hours.
In case of the determination at "hot," the solutions were boiled under a reflux
condenser for 18 hours.
QUININE HYDROCHLORIDE C20H24N2O2.HC1.2H2O.
SOLUBILITY IN AQUEOUS SALT SOLUTIONS AT 16°.
(Tarugi, 1914-)
The determinations were made by adding an aqueous solution of quinine
hydrochloride to the aqueous salt solution until turbidity occurred. From the
volumes involved, the solubility per 100 cc. was calculated.
In Aq.
NaCl.
In Aq.
NaNO3.
In Aq
.KC1.
In Aq
. CaCl2.
Gms. per 100 cc. Sol. -
Gms. per
100 CC. Sol.
Gms. per 100 cc. Sol.
Gms. per
TOO cc. Sol.
' NaCl.
Q.HCl.'
NaN03.
Q.HCl. '
' KC1.
Q.HCl.
'CaClj.
Q.HCl.
2.02
2.6
0.677
2-85
2.63
2-545
6-37
1.028
2.49
1.94
0.970
1.96
3
1.882
7-03
0.951
3-40
1.22
2.008
0.67
5-57
0.804
7-75
0.879
8-34
0-54
3-65
o-43
8.26
o.53i
7.96
0.765
11.40
0.205
9-31
o. 292
10.42
0.407
34-42
0.183
I5-56
o. 140
19. 12
0.168
17.87
0.205
y
19.83
0.085
3I-78
0.0663
25-74
0.0997
(Squire and
Caines,
1905-)
100 cc. 90% alcohol dissolve 20 gms. Q. bihydrochloride at I5°-2O°.
chloroform " 14.3 "
90% alcohol " 14.3 " Q.hydrochlorosulfateati5°-20°.
0-5 " Q- glycerophosphate at I5°-2O°.
100 gms. H2O dissolve 1.3 gms. anhydrous Q. glycerophosphate at 100°.
(Rogier and Fiore, 1913.)
QUININE SALICYLATE CMH24N2O2,C6H4(OH)COOH.2H2O.
SOLUBILITY IN AQUEOUS ALCOHOL AT 25°.
(Seidell, 1909, 1910.)
Wt. %
C2HBOH
in Solvent.
da Of
Sat. Sol.
Gms. Q. Sal.
2H2O per 100
Gms. Sat. So)
o
0.999
0.065
IO
0.982
0.080
20
0.966
0. 20O
30
0.952
0.48
40
0.935
i
50
0.916
1.70
Wt. %
C2H8OH
in Solvent.
&* of
Sat. Sol.
Gms. Q. Sal.
2H2O per loo
Gms. Sat. Sol.
60
0.896
2-45
70
0.876
3-25
80
0.854
4.20
90
0.832
4.71
92.3
0.826
4.62
100
0.797
3-15
579 QUININE SULFATE
SOLUBILITY OF QUININE SULFATE IN SEVERAL SOLVENTS AT 25°.
»(Schaefer, 1913.)
s . Cms. Q. Sulfate Solvent Cms. Q. SuUate
bolvent. per 1QQ cc Solvent. per 100 cc. Solvent.
Ethyl Alcohol 0.4 i vol. C2H5OH+4 vols. CHC13 12.5
Methyl Alcohol 3.12 i vol. C2H6OH+4 vols. CeHe o . 53
Chloroform 0.27 i vol. CH3OH+4 vols. CHC13 20
Benzene insol. i vol. CH3OH+4 vols. CeHe 4-76
100 gms. trichlorethylene dissolve 0.07 gm. Q. sulfate at 1 5°. (Wester and Bruins, 1914-)
QUININE TANNATES True and False
SOLUBILITY IN WATER AND IN AQUEOUS HC1 AT 37°. (Muraro, 1908.)
Gms. Q. Tannate per 100 Gms.
Tannate. Formula. ' »_ rC7 A., .m
H20. ?Jci% HCi
True Tannate I C2oH24N2O2.CioHi4O9.4H2O o 0.984 3-656
True Tannate II (C2oH24N2O2)2.(CioHi4O9)3.8H2O o 1.210 4.756
False Tannate (C2oH24N2O2.H2SO4)2(C1oH14O9)5.i4H2O 0.313 0.847 1.560
The work of Muraro is criticized by Biginelli (1908).
IOO cc. 90% alcohol dissolve 33.3 gms. Q. tannate at I5°-2O°. (Squire and Caines, 1905.)
QUININE PYROTARTRATES /, i, d.
SOLUBILITIES IN ALCOHOL AT 18°. (Ladenburg and Herz, 1898.)
ioo gms. alcohol dissolve 15 gms. of the / pyrotartrate, 3.2 gms. of the i and
4.2 gms of the d compound. The results show that the i acid is not a mixture of d
and / acid, and, therefore, that the i quinine compound is a salt of the racemic acid.
SOLUBILITY OF QUININE AND OF QUININE SALTS IN WATER AND OTHER
SOLVENTS. (U. s. P. vm.)
Gms. Quinine Compound per ioo Gms. Solvent in:
Compound. Water. Alcohol. Ether. Chloroform. Glycerol.
At 25°. At 80°. At 25°. At 25°. At 25°. At 25°.
C20H24N2O2 0.057 0.123 166.6 22.2 52.6 0.633
C2oH24N2O2.3H2O 0.065 0.129 166.6 76.9 62.5 0.472
C2oH24N2O2HC1.2H2O 5-55 250 166.6 0.417 122 12.2
C20H24.N202.CeH4(OH).-
COOH.|H2O 1.30 2.86 9.09 0.91 2.70 6.25
(C20H24N2O2)2.H2SO4.7H2O 0.139 2-22 1-16 ... 0.25 2.78
C20H24N2O2.H2SO4.7H2O n-77 *47 5-55 0.056 0.109 5-55
C20H24N2O2.HBr.H2O 2.5 33.3 149.2 6.2 12.5
QUINOLINE ETHIODIDE C9H7N.C2H5l.
IOO gms. H2O dissolve 301.3 gms. C9H7N.C2H5I at 25°. (Peddle and Turner, 1913.)
ioo gms. CHC13 dissolve 1.78 gms. C9H7N.C2H6I at 25°.
RADIUM EMANATIONS
SOLUBILITY IN WATER. (Boyle, 1911; Kofler, 1913.)
Solubility. Solubility.
L- , * v t°. , * X
/(Boyle). a (Kofler). /(Boyle). a (Kofler).
o 0.508 0.54 30 0.195 0.205
5 0.41 0.442 40 0.16 0.165
10 0.34 0.37 50 ... 0.14
15 0.29 0.31 60 ... 0.12
20 0.245 0.265 70 ... O.II
25 0.215 0.232 90 ... 0.108
The results of Boyle are in terms of /, the Ostwald Solubility Expression (see
V — v E'
p. 227). Those of Kofler are in terms of the expression a = =, where
V JtL
V and v are the volumes involved and E' and E the total amount of emanation
contained respectively in the air and in the liquid.
RADIUM EMANATIONS
58o
SOLUBILITY IN SEVERAL SOLVENTS.
(Ramstedt, 1911; Swinne, 1913.)
Results at o".
Results at 18°.
Results at 14°.
Solvent.
(Boyle, 1911.)
A).
Sp. Gr. of Sol.
/18-
Sp. Gr. of Sol.
IM
Water
0.52
0.9999
0.285
0.9986
0.30
Sea Water
. . .
. . .
0-255
Ethyl Alcohol
8.' 28
0.8065
6.17
0.7911
7-34
Amyl Alcohol
9-31
Acetone
7-99
0.8186
6.30
0.7972
Aniline
4-43
1.0379
3-80
I.O2IO
• . •
Benzene
12.82
0.8811
Carbon Bisulfide
33-4
1.2921
23.14
i . 2640
Chloroform
20.5
1.5264
15.08
1.4907
...
Cyclohexane
18.04
0.7306
.
Ethyl Acetate
9.41
0.9244
7-34
0.9029
...
Ethyl Ether
20.9
0.7362
15.08
0.7158
Glycerol
. . .
O.2I
i. 262
... •
Hexane
23-4
0.6769
16.56
0.6612
. . .
Toluene
18.4
0.8842
13.24
0.8666
13-7
The above results are in terms of the Ostwald Solubility Expression (see p. 227).
RESORCINOL
C6H4(OH)2
!» 3-
SOLUBILITY IN:
Water.
Ethyl Alcohol.
(Speyers — Am. J. Sci. [4]
14, 294, '02.)
(Speyers.)
to Sp.Gr.of Gms.C6H4(OH)2penooGms. So.Gr.of
Gms. CeH4(OH)2 per 100 Gms.
solutions
• * Water.
Solution. Solutions.
Alcohol.
Solution.
0
.101
60
37-5 1-033
2IO
67.8
10
.118
81
44-8
•036
223
69.0
20
•134
103
5o-7
.041
236
70-3
25
.142
117
53-9
•045
243
70.8
30
.148
56.7
.048
250
71.4
40
•J57
161
.056
266
72.7
50
.165
198
66.5
•065
286
74-1
60
.172
246
71.1
•075
311
75-7
70
1.176
320
76.2
.087
34i
77-3
80
I.I79
487
82.9
.104
375
78-9
NOTE. — The original results of Speyers are given in terms of mols. per 100
mols. H2O.
According to Vaubel (1895), 100 gms. H2O dissolve 175.5 gms. C6H4(OH)2,
or 100 gms. sat. solution contain 63.7 gms. at 20°. Sp. Gr. of sol. = 1.1335.
SOLUBILITY OF RESORCINOL IN ALCOHOLS AND IN ACIDS.
(Timofeiew, 1894.)
Solvent.
t°.
Gms. C6H4(OH)2 m
per 100 Gms.
Solvent.
t°.
Gms. C6H4(OH)2 m
per 100 Gms.
Sat. Sol.
Sat. Sol.
Methyl Alcohol
ii. 6
69
Formic Acid
15
29.2
Ethyl
10.4
59-2
Acetic
15
32.5
<< ii
ii. 6
61.5 •
Propionic "
15
22.8
Propyl "
10.4
51-5
Butyric
i5
14.7
<< «
ii. 6
51-6
Isobutyric "
15
9.6
«
Valeric
15
6-5
581 RESORCINOL
SOLUBILITY OF RESORCINOL IN BENZENE.
(Rothmund, 1898.)
to Cms. C6H4(OH)2 j.o Cms. CgH^OHJj
per 100 Cms. Sat. Sol. per 100 Cms. Sat. Sol.
73 3-i8 95.5 61.7
77 4-75 96.5 77-64
82 6.94 83.46 98.5
95.5 37.44 90.23 100
Between the concentrations 37.44 and 61.7 at 95.5° two liquid layers are
formed. The reciprocal solubilities of these two layers, determined by the
synthetic method (see Note, p. 16), are as follows:
Cms. C6H4(OH)2 per 100 Cms. Gms. CjH4(OH)2 per 100 Cms.
60
70
80
C6Hg Layer.
4.8
6.6
9.2
C6H4(OH)2 Layer.
79-4
77-5
75
90
IOO
105
C6Hg Layer.
13
19-5
24.6
C6H4(OH)2 Layer.
71-3
65.7
60.7
109.3 cnt- temp. 42.4
Resorcinol mixes with pyridine in all proportions. (Dehn, 1917.)
loo gms. aqueous 50% pyridine dissolve 901 gms. C6H4(OH)2wat2O0-25°.
IOO cc. olive oil dissolve 4.55 gms. C6H4(OH)2 m at I5°-2O°. (Squire and Caines, 1905.)
The coefficient of distribution of resorcinol at 25° between olive oil and water
(cone, in oil -5- cone, in H2O) is given as 0.04 by Boeseken and Waterman (1911,
1912).
Freezing-point data (solubility, see footnote, p. i), for mixtures of resorcinol
and p toluidine are given by Philip and Smith (1905) and by Vignpn (1891).
Results for mixtures of resorcinol and m xylene are given by Campetti (1917).
DISTRIBUTION OF RESORCINOL BETWEEN WATER AND ORGANIC
SOLVENTS AT ORDINARY TEMPERATURE.
(Vaubel — J. pr. Ch. [2] 67, 4?8, '03.)
Gms. Gms. CaH4(OH) in:
Solvents. Organic
Used. H20 Layer, g^^* Layer
1.191 60 cc. H2O+ 30 cc. Ether 0.2014 0.9896
1.191 60 cc. H2O-f 60 cc. Ether 0.2475 0.9525
0.800 40 cc. H2O + 40 cc. Benzene °-5^73 0-2127
0.800 40 cc. H2O-f 80 cc. Benzene 0.5773 0.2227
0.500 50 cc. H2O+ 50 cc. CC14 0.4885 0.0115
0.500 50 cc. H2O+ioo cc. CC14 0.4880 0.0120
0.500 50 cc. H2O+i5o cc. CC14 0.4880 0.0120
RHODIUM SALTS. SOLUBILITY IN WATER.
(Jorgensen — J. pr. Ch. [2] 27, 433, '83; 34, 394, '86; 44, SL '91-)
Salt. Formula
Chloro Purpureo Rhodium Chloride ClRh(NH3)5Cl2 17 0.56
Luteo Rhodium Chloride Rh(NH3)6Cl3 8 13.3
Luteo Rhodium Nitrate Rh(NH3)6(NO3)3 ord. t 2.1
Luteo Rhodium Sulphate [Rh(NH3)6]2(SO4)3.5H2O 20 2.3
ROSANILINE C20H21N3O.
IOO gms. H2O dissolve 0.03 gm. CaoH^NaC^ at 2O°-25°. (Dehn, 1917.)
loo gms. pyridine dissolve 41.5 gms. C2oH2iN3O4 at 2O°-25°. "
100 gms. aq. 50% pyridine dissolve 35.1 gms. C2oH2iN3O4 at 2O°-25°. "
ROSANILINE 582
Triphenyl p ROSANILINE HYDROCHLORIDE
SOLUBILITY IN SEVERAL SOLVENTS AT 23°.
(v. Szathmary de Szachmar, 1910.)
Solvent.
Methyl Alcohol
Ethyl
Amyl
Acetone
Aniline
Cms. Triphenyl p
Rosaniline HC1 per
100 Cms. Sat. Sol.
0.447
0.285
O.II
O.SI8
ROSOLIC ACID C20Hi603.
100 gms. H2O dissolve 0.12 gm. C2oHi6O3 at 2O°-25°.
100 gms. pyridine dissolve 160 gm. C^HieOa at 2O°-25°.
100 gms. aq. 50% pyridine dissolve 80 gm. C2oHi6O3 at 2O°-25°.
(Dehn, 1917.)
•UBIDIUM ALUMS.
See also Alums, p.
32.
SOLUBILITY IN
WATER.
(Locke, 1901.)
Gms. Alum per 100 Gms. H2O.
Ali
t °
Alum.
rormula.
Anhydrous.
Hydrated.
G. Mols.
Rb. Aluminum
Alum
RbAl(S04)2.i2H2O
25
I.8i
3.15
0.0059
3°
2.19
0.0072
35
2.66
. . .
0.0087
40
3.22
. .
0.0106
Rb.Chr
omium
Alum
RbCr(S
04)2.i2H20
25
2-57
4-34
0.0079
i
30
3-17
o. 0096
35
4.11
. . .
0.0128
tt
40
5-97
0.0181
Rb. Vanadium
Alum
RbV(SO4)2.i2H2O
25
5-79
9-93
0.0177
Rb. Iron Alum
RbFe(SO4)2.i2H2O
•25
9-74
16.98
0.0294
«
«
30
20.24
0.0617
Biltz and Wilke, 1906, find for the solubility of rubidium iron alum in water,
at 6.6°, 4.55 gms. per 100 cc. solution; at 25°, 29 gms; and at 40°, 52.6 gms.
RUBIDIUM FLUOBORIDE RbBF.
100 gms. H2O dissolve 0.55 gm. RbBF4 at 20°, and I gm. at 100°. (Godeffroy, 1876.)
RUBIDIUM BROMIDE RbBr.
SOLUBILITY IN WATER.
(Rimbach, 1905.)
Gms. RbBr per 100 Gms.
0-5
5
16
Gms. RbBr per 100 Urns.
Water.
I3I-85
Solution.
56.87
60.39
67.24
Water. Solution.
89.6 47.26 39.7
98 49-5° 57-5 i52-47
104.8 51.17 113.5 205.21
Freezing-point data for RbBr -f AgBr are given by Sandonnini (i9!2a).
RUBIDIUM BiCARBONATE RbHCO3.
100 gms. sat. solution in H2O contain 53.73 gms. RbHCO3 at about 20°.
(de Forcrand, 1909.)
RUBIDIUM CARBONATE Rb2CO3.
100 gms. absolute alcohol dissolve 0.74 gm. Rb2COs. (Bunsen.)
583
RUBIDIUM CHLORATE
RUBIDIUM CHLORATE RbClO3.
SOLUBILITY IN WATER.
(Calzolari, 1912.)
t o Cms. RbClO3 per f0 Gms. RbClO3 per
100 Cms. H2O. 100 Cms. H2O.
o 2.138 42.2 12.48
8 3.07 50 15.98
19.8 5.36 76 34-12.
30 8 99 62.8
There is some uncertainty as to whether the results of Calzolari refer to 100
gms. of H2O or 100 gms. of saturated solution.
100 gms. H2O dissolve 3. i gms. RbClO3at 15° (d^ of the sat. sol. = 1.07). (Carlson, '10.)
For earlier data see Reissig, 1863.
RUBIDIUM PerCHLORATE RbC104.
SOLUBILITY IN WATER.
(Carlson, 1910; Calzolari, 1912.)
Gms. RbClC-4 per 100 Gms. H2O.
Gms. RbC104 per 100 Gms. H2Q
I .
(Calzolari.)
(Carlson.)
i .
(Calzolari.)
(Carlson.)
0
°-5
I.I (l.007)
SO
3-5
4.6
10
0.6
1.2
60
4-85
6.27 (1.028)
20
i
1.56 (i.oio)
70
6.72
8.2
25
1.2
1.8
80
9.2
11.04 (i -°5°)
30
40
i-5
2-3
2.2
3.26 (I.OI7)
90
IOO
12.7
18
iS-5
22 (?) (1.070)
The figures in parentheses are densities of sat. solutions.
IOO gms. H2O dissolve 1.08 gm. RbClO4 at 21.3°.
(Longuimine, 1862.)
RUBIDIUM Potassium PerCHLORATE Rb2K(ClO4)3.
100 gms. sat. solution in H2O contain 1.55 gms. Rb2K(ClO4)3 at 20° (d20 of the
sat. solution = I.OI3).
RUBIDIUM CHLORIDE RBC1.
SOLUBILITY IN WATER.
(Rimbach, 1902; Berkeley, 1904.)
(Carlson, 1910.)
A. O
Mols. RbCl
Gms. RbCl
: rjer 100 Gms.
to
Mols. RbCl
Gms. RbCl
per 100 Gm
fc .
per Liter.
Water.
Solution.
•
per Liter.
'Water.
Solution.
O
5.17
77-o
43-5
60
6.90
115.5
53-6
10
5-55
84-4
45-8
70
7-12
121 .4
54-8
20
5-83
9I.I
47-7
80
7-33
127.2
56.0
30
6.17
97-6
49-4
90
7-52
I33-I
57-i
40
6-43
103-5
5°-9
IOO
7.71
138.9
58-9
50
6.67
109.3
52 .2
112.9
7-95
146.6
59-5
The following determinations of the Sp. Gr. of the sat. solutions are given by
Berkeley.
t°.
Sp. Gr.
0.55
1.4409
18.7
1.4865
60.25
1.5558
75-iS
1.5746
89.35
1.5905
"4
1.6148
31.5 44-7
1.5118 1.5348
* Boiling-point.
IOO gms. methyl alcohol dissolve 1.41 gms. RbCl at 25°. (Turner and Bissett, 1913.)
ethyl 0.078 gm.
propyl 0.015 " " "
" amyl 0.0025 " " " " " "
loo cc. anhydrous hydrazine dissolve 5 gms RbCl at room temp.
(Welsh and Broderson, 1915.)
Freezing-point data (solubility, see footnote, p. i) for RbCl + AgCl and
RbCl + T1C1 are given by Sandonnini (1911, 1914). Results for RbCl + NaCl
are given by Zemcznzny and Rambach (1910).
RUBIDIUM CHLORIDE 584
RUBIDIUM TELLURIUM CHLORIDE Rb2TeCl6.
loo gms. aq. HC1 of 1.2 Sp. Gr. dissolve 0.34 gm. Rb2TeCle at 23°.
100 gms. aq. HC1 of 1.05 Sp. Gr. dissolve 13.09 gms. Rb2TeCl6 at 23°.
(Wheeler, 1893.)
RUBIDIUM THALLIUM CHLORIDE 3RbClTlCl3.2H2O.
100 gms. H2O dissolve 13.3 gms. at 18°, and 62.5 gms. at 100°. (Godeffroy, 1886.)
RUBIDIUM CHROMATE (Mono) Rb2CrO4.
SOLUBILITY IN WATER.
(Schreinemakers and Filippo, Jr., 1906.)
Gms. RbCrO4
t°. per loo Gms.
Solution.
50 47-44
60 . 4 48 . 90
Solid Phase, Ice
-0.6 0.95
— i.i 7.22
-1.57 9.87
EQUILIBRIUM IN THE SYSTEM RUBIDIUM OXIDE, CHROMIUM TRIOXIDE AND
WATER AT 30°.
(Schreinemakers and Filippo, Jr., 1906.)
Gms. RbCrO4
t°.
per 100 Gms.
Solution.
- 7
36.65
o
38.27
10
40.23
20
42.42
30
44.11
40
46.13
Gms. RbCrO4
t°. per zoo Gms.
Solution.
— 2.40
I5-58
-3-25
-4.14
20.03
24.28
-5-55
-6.7I
about —7
30.15
34-3i
36.65
Gms. per 100 Gms. Sat. Sol.
Cr03.
Rb2O.
O
60.56
O
56.82
0.776
37-88
2.89
34.89
4.96
30.20
8-54
28.17
11.98
27.99
15-38
28.73
15-54
28.55
13.69
23.87
9.98
17.56
5-72
8.47
4.58
7.98
4.87
4.60
8.16
3-57
Solid Phase.
RbOH
Gms. per 100 Gms. Sat. Sol.
Cr03. Rb,0. '
13.91 3.38
15-05 3-45
15-31 3-59
15.19 3-I9
18.96 2.37
24.92 1.66
37-34 i-6i
48 . 20 i . 54
53-87 1-67
54.29 1.28
58.69 1.07
62.38 0.93
62.74 0.93
63.07 0.92
62.28 o
RUBIDIUM DICHROMATE Rb2Cr3O7.
SOLUBILITY OF THE POLYMORPHIC FORMS IN WATER.
(Stortenbecker, 1907; see also Wyrouboff, 1901.)
Solid Phase.
+Rb2Cr3010
RbjCrAs
" +Rb2Cr207
RfcCrA
" +Rb2CrA,
Rb2Cr4Oi3
+CrO,
Cr03
Gms. Rb2Cr3O7 per too Gms. Sat. Sol.
18
24
30
40
50
65
Monoclinic Form.
5-42
6-94
9.08
13.22
18.94
28.10
Triclinic Form.
4.96
6-55
8.70
12.90
18.77
27.30
+s l \j
loo gms. sat. aq. solution contain 9.47 gms. Rb2O2O7, at 30°.
(Schreinemakers and Filippo, Jr., 1906.)
RUBIDIUM FLUORIDE RbF.iiH2O.
100 gms. H2O dissolve 130.6 gms. RbF at 18°.
(de Forcrand, 1911.)
585 RUBIDIUM HYDROXIDE
RUBIDIUM HYDROXIDE RbOH.
100 gms. sat. aqueous solution contain 63.39 £ms- RbOH at 30°.
(Schreinemakers and Filippo.igoG.)
100 gms. sat. aqueous solution contain 64.17 gms. RbOH at 15°. (de Forcrand, igoga.)
Fusion-point data for mixtures of RbOH + NaOH are given by (v. Hevesy,
1900).
RUBIDIUM IODATE RbIO3.
100 gms. H2O dissolve 2.1 gms. RbIO3 at 23°. (Wheeler, 1892.)
RUBIDIUM PerlODATE RbIO4.
100 gms. H2O dissolve 0.65 gm. RbIO4 at 13°, dig. of sat. solution = 1.0052.
(Barker, 1908.)
RUBIDIUM IODIDE Rbl.
100 gms. H2O dissolve 137.5 gms- Rbl at 6.9°, and 152 gms at 17.4°.
(Reissig, 1863.)
SOLUBILITY OF RUBIDIUM IODIDE IN ORGANIC SOLVENTS.
(Walden, 1906.)
Acetonitrile
Propionitrile
Nitromethane
Acetone
Furfurol
CH3CN
C2H5CN
CH3N02
(CH3)2CO
C4H3O.COH
1.478 at o°
0.274 "
0.567 "
0.960 "
i. 350 at 25°
0-305 "
0.518 "
0.674
4-930
Fusion-point data for Rbl + Agl are given by Sandonnini (i9i2a).
RUBIDIUM PerlODIDES
SOLUBILITY IN WATER AT 25°.
(Foote and Chalker, 1908.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
'-RbL ' I— Sohd Phase. ^^ — Sohd Phase.
61.93 ° Rbl 28.01 64.85 RbI3+I
59.94 5.90 " +RbI3 27.85 65.12
57.24 8.02 Rbi3 27.83 65.13
33.89 38.08 27.99 64.98
The results show that Rbly and Rblg are not formed.
RUBIDIUM BROMIODIDE RbBr2I.
100 gms. sat. aq. solution contain about 44 gms. RbBr2I, and the Sp. Gr. of
the solution is 3.84. (Wells and Wheeler, 1892.)
RUBIDIUM IRIDATE and IRIDITES
SOLUBILITIES IN WATER.
(Delepine, 1908.)
Salt. Formula. t°. i^Gms^lfo
Rubidium Chloroiridate Rb2IrCle 19 0.0555
Tri rubidium Hexachloroiridite RbalrCle.H^O 19 0.91
Dirubidium Aquopentachloroiridite Rb2IrCl5(H2O) 19 1.05
RUBIDIUM ParaMOLYBDATE 5Rb2O.i2MoO3.H2O.
100 cc. sat. aq. solution contain 1.941 gms. of the salt at 24°. (Wempe, 1912.)
RUBIDIUM NITRATE 586
RUBIDIUM NITRATE RbNO3.
SOLUBILITY IN WATER.
(Berkeley, 1904.)
Mols. Grams RbNO3 per 100 Gms. RbNO Gms- RbNO3-per 100 Cms.
Per Liter. Water. Solution. Per Liter. Water. Solution.
O I-27 19.5 16.3 60 7.99 200 66.7
10 2.04 33-o 24.8 70 9.02 251 71.5
20 3.10 53.3 34-6 80 9.93 309 75.6
30 4-34 81.3 44-8 90 10.77 375 7^-9
40 5.68 116.7 53.9 100 n-54 452 81.9
50 6.88 155-6 60.9 118.3 12.76 617 86.1
The following Sp. Gr. determinations are also given by Berkeley.
t°. 0.6 15.85 31.55 45.85 63.4 75.60 90.95 118.3*
Sp. Gr. Sat. Sol. 0.1389 1.2665 1.4483 1.6216 1.8006 1.9055 2.0178 2.1867
* Boiling-point.
THE SOLUBILITY AND SUPERSOLUBILITY ICE CURVES FOR RUBIDIUM NITRATE
AND WATER.
(Jones, 1908.)
Gms. RbNO3 per 100 Gms. H2O. Gms. RbNO3 per 100 Gms. H2O.
of Ice. Solubility Supersolubility of ice> ' Solubility Supersolubility
Curve. Curve. Curve. Curve.
-0.4 1.16 ... -3-5 ••• 9-94
-1.8 ... 1.24 -2.3 13.97
-2.1 5.39 -4.2 ... 13.97
— 1.7 9.94 ... — 2 . 7 Cryohydrate 17.11
RUBIDIUM Telluric Acid OXALATE Rb2[H6TeO6.C2O4].
SOLUBILITY IN WATER.
(Rosenheim and Weinheber, 1910-11.)
t°. 0° 20° 30° 40° 50°
Gms. Rb2[H6Te06.C2O4] per zoo gms. H2O 3.85 7.26 9.40 12.76 16.90
RUBIDIUM PERMANGANATE RbMnO4.
One liter of aqueous solution contains 6.03 gms. RbMnO4 at 7°.
(Muthmann and Kuntze, 1894.)
100 cc. sat. aq. solution contain 0.46 gm. RbMnO4 at 2°, 1.06 gms. at 19° and
4.68 gms. at 60°. (Patterson, 1906.)
RUBIDIUM SELENATE Rb2SeO4.
100 gms. H2O dissolve 158.9 gms. Rb2SeO4 at 12°. (Tutton, 1897.)
SOLUBILITY OF MIXED CRYSTALS OF RUBIDIUM ACID SELENATE AND RUBIDIUM
ACID TELLURATE AND OF RUBIDIUM ACID SULFATE AND RUBIDIUM ACID TEL-
LURATE IN WATER AT 25°. (Pellini, 1909.)
Results for RbHSeO4 + RbHTeO4. Results for RbHSO4 + RbHTeSO4.
Gms. per loop cc. Sat. Sol. Mol. % Selenate Gms. per loop cc. Sat. Sol. Mol. % Sulfate
RbHSe04. RbHTe04. in Solid Phase. 'RbHSO4. RbHTeO4'. in Solid Phase.
76.46 39.51 51.55 26.675 38.403 47-91
95-82 35.30 52.22 32.117 31.58 50.33
171.70 22.98 53.95 42.917 26.764 50.74
462.80 5 56.33 59.074' 20.182 50.99
859-30 3.40 67. 46* 498.25 0.02887 52.52
RUBIDIUM FLUOSILICATE Rb2SiF6.
100 gms. H2O dissolve 0.16 gm. Rb2SiF6 at 20°, and 1.36 gms. at 100°.
(Stolba, 1867.)
RUBIDIUM SILICOTUNGSTATE Rb8SiWi2O42.
100 gms. H2O dissolve 0.65 gm. RbsSiW^O^ at 20°, and 5.1 gms. at 100°.
(Godeffroy, 1876.)
587 RUBIDIUM SULFATE
RUBIDIUM SULFATE Rb2SO4. SOLUBILITY IN WATER.
SOLUBILITY IN WATER.
(Etard, 1894; Berkeley, 1904.)
Gms.
I .
per Liter.
Water.
Solution.
ii .
per Liter.
Water.
Solution.
0
1.27
36-4
27-3
60
2.IS
67.4
40-3
10
I .46
42 .6
29.9
70
2.25
71.4
41.7
20
I .64
48.2
32-5
80
2-34
75 -°
42.9
30
1-79
53-5
34-9
90
2.42
78.7
44.0
40
1.92
58-5
36-9
100
2.49
81.8
45-o
SO
2.04
63.1
38-7
IO2 .4
2 .50
82.6
45-2
The following Sp. Gr. determinations are also given by Berkeley.
t°. 0.5 15.80 31.6 44.2 57-90 74-75 89.45 102.4*
Sp.Gr.Sat.Sol. 1.2740 1.3287 1.3704 1.3998 1.4232 1.4480 1.4649 1-4753
* b. pt.
100 cc. sat. solution in absolute H2SO4 contain 58.81 gms. Rb2SO4.
(Bergius, 1910.)
SOLUBILITY OF RUBIDIUM DOUBLE SULFATES IN WATER AT 25°
(Locke, 1902.)
Per IPO cc. H2O. Per 100 cc. H2O.
Formula. ' Gms. Mols. Formula. ' Gms. " Mols.
Anh. Salt. Salt. Anh. Salt. Salt.
Rb2Cd(SO4)2.6H2O 76.7 0.1615 Rb2Mn(SO4)2.6H2O 35.7 0.0857
Rb2Co(SO4)2.6H2O 9.28 0.022 Rb2Mg(SO4)2.6H2O 20.2 0.0521
Rb2Cu(SO4)2.6H2O 10.28 0.0241 Rb2Ni(SO4)2.6H2O 5.98 0.0142
RblFefSO4)2.6H2O 24.28 0.0579 Rb2Zn(SO4)2.6H2O 10.10 0.0236
RUBIDIUM Dihydroxy TARTARIC ACID
100 gms. H2O dissolve 6.51 gms. Rb2C4H4O8.3H2O at o°. (Fenton, 1898.)
On account of the unstable character of the compound, only \ hour was allowed
for saturation of the solution.
RUTHENIUM SALTS
SOLUBILITIES IN WATER.
(Howe, 1894.)
Salt.
Formula.
t°.
Gms. Salt
per 100 Gms.
H20.
Ruthenium Potassium Nitrosochloride
K2RuCl5NO
25
12
it
tt it
(i
00
80
tt
Ammonium Nitrosochloride
(NH4)2RuCl5NO
25
5
n
« n
tt
00
22
ti
Rubidium Nitrosochloride
Rb2RuCl5NO
25
o-57
(i
a it
u
60
2.13
tt
11 (hydrated)
Rb2RuCl5NO.2H2O
25
114-3
(i
Caesium Nitrosochloride
Cs2RuCl5NO
25
O.2O
n
it tt
tt
60
0.56
n
11 " (hydrated)
Cs2RuCl5.NO.2H2O
25
105.8
SACCHARIN (i, Benzosulfonazole, 2(1), one) C6H4<cQ2>NH.
100 parts H2O dissolve 0.4 part at 25° and 4.17 parts at 100°.
100 parts alcohol dissolve 4 parts at 25°. (U. S. P. VTH.)
loo gms. trichlorethylene dissolve 0.012 gm. saccharin at 15°.
(Wester and Bruins, 1914.)
SACCHARIN 588
DISTRIBUTION OF SACCHARIN AT 25° BETWEEN:
Water * and Ether. Water f and Amyl Acetate.
(Marden, 1914.) (Marden, 1914.)
Gms. Saccharin per: Gms. Saccharin per:
'loocc. H20 50 cc. Ethe? Dist> CoeL 105 cc. Aq. 50 cc. AmyP Dist> Coef'
Layer. Layer. Layer. Acetate Layer.
0.0290 0.0438 0.267 0-0045 0.0700 0.0306
0.0458 0.0829 0.235 0.0065 0-0957 0.0322
0.0719 0.1245 0.245 O.OII4 0.1724 0.0315
* Slightly acidified with HC1. f Containing 5 cc. cone. HC1 per 100 cc.
The amount of saccharin entering the ethereal layer is increased by addition
of HC1 to the aqueous layer. With 5 cc. cone. HC1 per 100 cc. H2O, the distribu-
tion coefficient is reduced to 0.0624.
SALICIN C6H4(CH2.OH)O.C6Hu05.
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent. f. GmS-SP0Tven?.GmS- Authority.
Water 15 3.52 (Greenish and Smith, 1903.)
Water 25 4.16 (Dott, 1907.)
90% Alcohol 15 1.5 (Greenish and Smith, 1903.)
90% Alcohol 15 2 (Squire and Caines, 1905.)
Trichlor Ethylene 15 O.OI3 (Wester and Bruins, 1914.)
SALICYLAMIDE OH.C6H4CONH2.
DISTRIBUTION BETWEEN WATER AND OLIVE OIL.
(Meyer, 1901.)
Gms. OHCeH^CONHz per 100 cc.
t°. , •*• v Dist. Coef.
H2O Layer. Oil Layer.
3 0.056 0.126 2.25
36 0.075 0.107 i-40
SALICYLIC ACID C6H4.OH.COOH'i:2.
SOLUBILITY IN WATER.
(Average curve from the closely agreeing determinations of Walker and Wood, 1898; at 26.4°, Philip,
1905; at 25°, Paul, 1894; at 20°, Hoitsema, i8g8a; Hoffman and Langbeck, 1905. For determinations
not in good agreement with the following, see Alexejew, 1886; Bourgoin, 1878; Ost., 1878.)
Gms.
Gms.
Gms.
to C6H4.OH.COOH
t°
C6H4.OH.COOH
t°
CsH^OH.COOH
Liter Solution.
per
Liter Solution.
Liter Solution.
0 0.8
25
2.2
60
8.2
IO 1.2
30
2-7
70
13.2
20 1.8
40
3-7
80
20.5
50
5-4
SOLUBILITY
OF SALICYLIC ACID IN
WATER
(Savorro, 1914.)
Gms.
Gms.
Gms.
t«, C6H4.OH.COOH
t°
C6H4.OH.COOH
t°
C6H4.OH.COOH
per 1000 Gms.
* .
per 1000 Gms.
i* .
per 1000 Gms.
Sat. Sol.
Sat. Sol.
Sat. Sol.
o 1.24
35
3-51
70
13.70
5 1-29
40
4.16
75
17-55
10 1.35
45
4.89
80
22.O8
15 1.84
6-38
85
27.92
20 2
55
7-44
90
37-35
25 2.48
60
9
95
50-48
30 2 . 98
65
10.94
100
75-07
589 SALICYLIC ACID
SOLUBILITY OF SALICYLIC ACID (LIQUID) IN WATER.
Determinations by Synthetic Method. See Note, p. 16. The original data
in each case were plotted and the following figures read from the curves.
(Flaschner and Rankin, 1910.)
(Alexejew.)
Cms. C«H4OHCOOH per
100 Cms.
Cms. C|H«OHCOOH per
100 Cms.
I .
Aqueous
Salicylic Acid
i .
Aqueous
Salicylic Acid
Layer.
Layer.
Layer.
Layer.
60
7
68
60
4-5
68
70
8
64
70
6-5
62.5
80
12
58
80
10
54
90
19
49
8$
15
46
95 crit
temp.
•_i _r
87 crit.
temp. 30
are also given by Flaschner and Rankin.
SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SALT SOLUTIONS AT 25° AND
AT 35°. (Hoffman and Langbeck, 1905.)
C6H4OH.COOH Dissolved at 25°. C8H4OH.COOH Dissolved at 35°.
Salt.
iNormaiiiy
of Salt
Solution.
oms. /-
Salt per
Liter.
Gms. per
1000 Gms.
Sat. Sol.
Gm. Mol.
Per cent.
Gms. per
1000 Gms.
Sat. Sol.
Gm. Mol.
Per cent.
KC1
0.020
I
.49
2.24
2.92l6.
io-4
3
•23
4
.2206.
io-4
u
O.IOO
7
.46
2.25
2-9377
tt
3
•23
4
.22O3
11
tt
0.492
36
•73
2.02
2.6321
tt
3
.01
3
.9268
tl
tl
1.004
74
•.92
1.89
2.4759
tt
2
.68
3
•5003
It
KN03
0.020
2
.02
2.25
3-9351
tt
3
•25
4
.2499
tt
«
O.IOO
10
.12
2.30
3.0103
tl
3
•32
4
•3334
11
tt
0.504
51
.10
2.38
3 . 1061
ft
3
.38
4
.4123
It
tt
I .OO4
101
.60
2-39
3.1249
tl
3
•36
4
.3848
It
NaCl
O.O2O
I
.19
2.23
2.9110
tl
3
.22
4
.2062
It
tt
O.IOO
5
•95
2.22
2.9027
tt
3
.20
4
.1806
tt
it
0.497
29
• 50
2
2.6128
tl
2
-85
3
.7171
tt
tt
0.988
58
.80
1.72
2.2487
tt
2
•43
3
.1596
tt
SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SALT SOLUTIONS AT 25°.
(Philip, 1905; Philip and Garner, 1909.)
In Aq. Sodium
Acetate.
Gms. per Liter.
CHjCOONa. C«H4OHCOOH.
i. oi 3.60
2-48 5-93
5-03 9-56
10.07 16.81
In Aq. Sodium
Succinate.
Gms. per Liter.
C,H4(COONa)2. C«H4OHCOOH.
1.18 2.97
2-93 4-34
5-85 6.56
11.73 10.82
In Aq. Sodium
Formate.
Gms. per Liter.
HCOONa. C«H4OHCOOH.
0.81 3.40
1.63 4-42
4.06 7.II
8.14 IO.44
In Aq. Potassium
Formate.
Gms. per Liter.
HCOOK.
0
1.03
2.56
In Aq. Sodium Monochlor
Acetate.
Gms. per Liter.
CH2ClCOONa. C^OHCOOH.
1.38 2.83
3-43 3-58
6 . 84 4 . 64
13.71 6.17
In Aq. Sodium Butyrate
at 26.4°.
Gms. per Liter.
C,H4OHCOOH. C,H7COONa. CgH^OHCOOI?.
2.265 i 3-3
3-38 2 4.5
4-93 4 6.85
7-13 * 8.1
One liter of I normal aqueous sodium salicylate solution dissolves 4.97 gms.
salicylic acid at 25°. (Sidgwick, 1910.)
SALICYLIC ACID
590
SOLUBILITY OF
SALICYLIC ACID IN
SALIC YLATE
(Hoitsema,
Gm. Mols. per Liter.
^OOH1"
QftOH-
COONa.
0.0132
0
O.OII2
0.017
0.0124
0.113
0.0143
0.226
0.0164
0-344
O.O2O3
0.500
O.O62
1.70
0.095
2. II
0.091
2.19
0.086
3-41
O.oSl
4-23
0.048
4.18
O.O2I
4.12
O.
4.15
Sp. Gr. of
Solutions.
.OO2
.003
.009
.016
.024
1-034
I. 112
1-137
I.I44
I.2I5
1.263
Cms. per Liter.
259
258
257
AQUEOUS SOLUTIONS OF SODIUM
AT 2O.I°.
Solid Phase.
Cs^OHCOOH
( C6H4OHCOOH.C6H4OHCOONa
( +C6H4OHCOOH
C6H4OHCOOH.C6H4OHCOONa
( C8H4OHCOOH.C8H4OHCOONa
| +C6H4OHCOONa
QH4OHCOONa
C6H4OH-
COOH.
QH4OH-
COONa.
1.823
0
1-55
I.7I
2.705
17-98
1.97
2.26
2.80
54-74
8.56
270.5
13.11
335 • 7
12.56
11.88
348.4
542.6
11.19
673
6.63
2.90
o
665.1
665.5
660.3
SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SOLUTIONS OF ACIDS AT 25°.
(Kendall, 1911.)
Gms. per Liter.
Gms. per Liter.
Acid.
*»• «-
Acid.
C.H.OH-
Water alone
o
2.257
Formic Acid
230
15
HCOOH 2.370
Acetic Acid
37.52CH3COOH
2-335
"
46O
30
" 2.901
"
75-05
"
2.409
Hydrochloric Acid
o
653
HC1 1 . 781
"
150. 10
"
2-549
«
I
302
1.710
u
300.20
"
2.850
«
A
558
"
•677
Formic Acid
2.38
HCOOH
2.114
"
9
117
" 3
•649
u
4-59
"
2-035
n
18
235
"
.551
tt
11.05
"
2.114
Malonic Acid
•?
253
CH2(COOH)2
.051
ft
21.17
"
2-035
«
10
49
"
•944
"
28.76
"
2.049
"
20
84
«
.880
"
57-53
"
2.066
Methyl Picric Acid
2
28
C7H607N, 2.115
"
115.07
u
2. 121
SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SOLUTIONS OF o NITROBENZOIC
Gms. per Liter.
O
2.615
7- 202
7.283
o C6H4-
OHCOOH.
2.257
1-974
1.887
1.885
ACID AT 25° AND VICE VERSA.
(Kendall, 1911.)
Gms. per Liter
Solid Phase. ' ~ „ XT
Salicylic Acid
+Nitrobenzoic
7.188
7.213
7-233
o C«H4.OH.-
COOH.
2.243
1.873
1.294
Solid Phase.
o Nitrobenzoic Acid
da of Sat. Sol.
SOLUBILITY OF SALICYLIC ACID IN AQUEOUS ALCOHOL AT 25°.
(Seidell, 1908, 1909, 1910.)
Wt. Per cent Gms.
C2H5OH in ^ Sat. Sol. C,H4OHCOOH
Solvent. per 100 Gms.
Sat. Sol.
10 0.984 0.38
2O 0.970 0.80
3° 0.959 2.20
40 0.951 5.90 90
SO 0.945 12.20 100 0.919 33-20
Wt. Per cent
QHsOH in
Solvent.
60
70
80
0-943
0.941
0-937
0.930
0.919
Gms.
C6H4OHCOOH
per 100 Gms.
Sat. Sol.
18.30
24
28.30
591
SALICYLIC ACID
SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL,
ISOBUTYL ALCOHOL, DEXTROSE, CANE SUGAR, AND OF LEVULOSE AT 25°
AND AT 35°. (Hoffmann and Langbeck, 1905.)
Cone, of Solvent.
C6H4OH.COOH Dissolved
at 25°.
Aq. Solvent.
Normal-
ity.
Gms. per
Liter.
Gm. Mol.
Per cent.
Gms. per
100 Gms.
Sat. Sol.
Gm. Mol.
Per cent.
Gms. per
100 Gms
Sat. Sol.
CjjHsOH
0.0249
I
.146
2
.8966.
io-4
O.222
4-
2044.
io-4
0.322
«
0.0560
2
•578
2
.9150
tt
0.223
4-
2348
11
0.324
cc
0.1747
8
.04
2
.9901
cc
O.229
.
tt
0.2399
II
•05
. . .
4-
434i
n
0-339
tt
1.03
47
•4
3
•5279
ct
O.27O
5-
2816
n
0.404
cc
1.638
75
•44
3
•9253
Cl
0.300
C^OH (iso)
0.020
i
.496
2
.909
cc
0.223
4-
229
Cl
0.324
cc
O.O5I
3
•74
2
•955
cc
O.226
4-
289
n
0.329
It
0. 100
7
.48
3
-033
ct
0.232
4-
435
"
0-339
cc
0.521
38
.60
3
.718
Cl
0.285
5-
624
tt
0.431
C6H1206
0.02
3
.6
2
.886
Cl
O.22I
4-
184
n
0.321
tt
O.IO
18
2
.898
Cl
0.222
4-
202
1C
0.322
tt
0.50
89
.6
2
•954
1C
O.226
4-
263
ct
0.326
tt
I
180
3
.015
11
0.231
4-
360
11
0-334
Ci2H22On
O.O2
6
.88
2
.902
1C
0.221
4-
206
Cl
0.322
tt
O.IO
34
•97
2
.964
cc
o. 227
4-
287
11
0.328
tt
0.50
172
3
•239
cc
0.248
4-
697
11
0.360
n
I.IO
376
•3
3
-633
1C
0.278
5-
236
11
O.40I
CeH1206
O.02
3
.6
2
.888
Cl
O.22I
.
. . .
cc
0.06
IO
.8
2
•895
1C
O.22I
. .
.
tt
0.25
45
2
•944
Cl
0.225
.
SOLUBILITY OF SALICYLIC ACID IN ALCOHOLS, IN ETHER AND IN ACETONE.
(Timofeiew, 1891; at 15°, Bourgoin, 1878; at 23°, Walker and Wood, 1898.) .
Solvent.
CH3OH
CH3OH
C2H5OH
C2H5OH
C2H5OH
C2H5OH 90%
Gms. C6H4OHCOOH
t°f per 100 Gms.
Solvent.
C3H7OH(w)
C3H7OH(n)
(CH3)20
(CH3)20
(CH3)2CO
Gms. C6H4OHCOOH
t°_ per loo Gms.
- 3
+ 21
— 3
+ 15
21
15
Solvent.
40.67
62.48
36.12
53-53
42.09
Solution.
28.91
38.46
26.29
33-17
34.87
29.62
- 3
+ 21
15
23
Solvent.
26. 12
37.69
50-47
Solution.
2O.7I
27.36'
33-55
23-4*
31-3*
Gms. per 100 cc. sat. sol. instead of per 100 gms. sat. sol.
100 gms. sat. solution in methyl alcohol contain 39.87 gms. salicylic acid at 15°.
(Savorro, 1914.)
SOLUBILITY OF SALICYLIC ACID IN MIXTURES OF ACETONE AND BENZENE AT 25°.
(Marden and Dover, 1917.)
Gms. per 100 Gms. Mixed Solvent. Gms. per 100 Gms. Mixed Solvent. Gms. per too Gms. Mixed Solvent.
Acetone.
IOO
00
80
70
Salicylic Acid.
55
4<U
42.3
Acetone.
Salicylic Acid.
Acetone.
Salicylic Acid.
60
36.7
20
15
50
31
10
7-1
40
25-3
0
0.92
3C
20
SALICYLIC ACID 592
SOLUBILITY OF SALICYLIC ACID IN BENZENE.
(Walker and Wood, 1898.) (von Euler and Lowenhamn, 1916.)
Gms. C«H4- Gms. C6H4- Gms. C6H4-
f0 OHCOOH to OHCOOH « Solvent OHCOOH
per goo Gms. per 100 Gms. per 100 cc.
c
eHe.
C6H6.
Sat. Sol.
II
• 7
0.
460
34
6
I.26l
18
CeH6
0.525
18
,2
0.
579
36.
6
1-430
25
CeH6
0.762
25
0.
78
49
4
2.380
18
o.5wCH2ClCqOHinC6H6
1.698
30
• 5
0.
991
64
2
4.40
18
o . 5^ C-gilsOJii. in C-gldLs
0.746
SOLUBILITY OF SALICYLIC ACID IN MIXTURES OF BENZENE AND ETHYL
ACETATE AT 25°.
(Harden and Dover, 1917.)
Cms, per 100 Gms. Mixed Solvent. Gms. per 100 Gms. Mixed Solvent. Gms. per 100 Gms. Mixed Solvent.
Ethyl Acetate. Salicylic Acid. Ethyl Acetate. Salicylic Acid. Ethyl Acetate. Salicylic Acid.
100 38 60 16.6 20 6.2
90 24.2 50 14.5 10 3-42
80 22.7 40 12.8 o 0.92
70 19-5 30 9-6
SOLUBILITY OF SALICYLIC ACID IN SEVERAL SOLVENTS AT 25°.
(Herz and Rathmann, 1913.)
SolvPr Gms. Cel^OHCOOH _, Gms. CeH4OHCOOH
Solvent. per zoo cc. Sat. Sol. Solvent' per 100 cc. Sat. Sol.
Chloroform 2.168 Tetrachlor Ethylene 1.105
Carbon Tetrachloride 0.4143 Tetrachlor Ethane 2.085
Trichlor Ethylene i-5*9 Pentachlor Ethane 1.064
100 gms. dichlor ethylene dissolve 0.757 gm. salicylic acid at 15°. ) (Wester and
loo gms. trichlor ethylene dissolve 0.28 gm. salicylic acid at 15°. J Bruins, 1914.)
SOLUBILITY OF SALICYLIC ACID IN OILS (Temp, not stated).
(Engfeldt, 1913.)
Gms. Gms.
Oil of- C6H4OHCOOH Oilof. C6H4OHCOOH
per 100 Gms. per 100 Gms.
Sat. Sol. Sat. Sol.
Phocae (Dog Fish Oil) i . 70 Sesami 2.61
Jecoris Aselli (Cod Liver Oil) i .-86 Cannabis 3
Arachidis (Peanut Oil) i . 88 Lini (Linseed Oil) 3 . 04
Amygdalarum 2.08 Juglandis (Walnut Oil) 3.15
Olivae (Olive Oil) 2 . 14 Gossypii (Cottonseed Oil) 3 . 23
Rapse (Rape Seed Oil) 2. 17 Ricini (Castor Oil) 12.98
Papaveris (Poppy Seed Oil) 2.22 Paraffiniam Liquid o
The ratio of the solubilities of salicylic acid in olive oil and in water (cone.
in oil -5- cone, in H^O) at 25° is given as n.8 by Boeseken and Waterman (1911,
1912). This corresponds to 2.6 gms. acid per 100 gms. olive oil.
DISTRIBUTION OF SALICYLIC ACID BETWEEN:
Water and Benzene. (Hendrixon, 1897.) Water and Chloroform. (Hendrixon, 1897.)
Results at 10°. Results at 40°. Results at 10°. Results at 40°.
Gms. Acid 100 cc. Gms. Acid per 100 cc. Gms. Acid per 100 cc. Gms. Acid^per 100 cc."
H20 Layer. QH, Layer. 'H2O Layer ' C6H6 Layer.' H2O Layer. CHC13 Layer! H2O Layer. CHC13 Layer.
0.0264 0.0391 O.O260 0.0400 0.0293 0.0442 0.0335 0.0475
0.0377
0.1200
0.1292
0.0655
0.4159
0.4713
O.O7I9
0.1220
0.1563
0.2014
0.1649
0-3539
0.50l6
0.7625
0.0457
o. 1172
0.1229
0.1236
o . 0946
0.5640
0.6196
0.6269
0.0819
0.1589
0.2687
0.3053
0.1775
0.5297
1.3887
1.7570
Similar data for the 'distribution between water and benzene at 18° are given
by Nernst (1891).
I/ .
H20 Rich Layer.
Acid Rich Layer.
25
4-8
50
6
74
70
10
67
80
14
00
85
17-5
55
87.5
20
50
89 crit.
temp. 35
593 SALICYLIC ACID
Acetyl SALICYLIC ACID (Aspirin) CH3COO.C6H4.COOH, 1.2.
SOLUBILITY AND MELTING-POINT CURVES FOR MIXTURES OF ACETYL SALICYLIC
ACID AND WATER, DETERMINED BY THE SYNTHETIC METHOD.
(Flaschner and Rankin, 1909.)
Solubility Curve (Liquid Acid+H2O). M.-pt. Curve (Solid Acid +H»O).
Cms. CH3COO.C6H4.COOH per 100 Cms. Cms. CHjCOOQHr
t°. COOH per too Cms.
Mixture.
82.4 4.8
90.4 10
92.4 20
93 . 6 60
99 80
109.4 89.5
131 100
SALOL (Phenylsalicylate) CeH^OH.COOCeHs, 1.2.
SOLUBILITY OF SALOL IN AQUEOUS ALCOHOL AT 25°. (Seidell, 1909, 1910.)
Wt. Per cent . * Gins. Salol Wt. Per cent . ni Gms. Salol
C,H6OHin of? ell per 100 Gms. C2H5OH in sit Sol per 100 Gms.
Solvent. Sat' SoL ' Sat. Sol. Solvent. Sat. Sol.
O 0.999 0.015 70 0.877 4.40
20 0.967 0.020 80 0.863 7-7°
40 0.934 0.22 90 0.865 *4
50 0.914 0.76 92.3 0.868 17-70
60 0.895 2-10 I0° 0.898 35
SOLUBILITY OF SALOL IN SEVERAL SOLVENTS. (Seidell, 1907.)
, a. Gms. Salol j oaf Gms. Salol
Solvent. t°. c, per 100 Gms. Solvent. t°. V>? t' per 100 Gms.
SoL Sat. Sol. bo1' Sat. Sol.
Acetone 30-31 ... 90 .99 Amyl Alcohol 25 0.869 20.44
Benzene 30-31 1.148 88.57 Acetic Acid (99. 5%) 21.5 1.143 63.24
Amyl Acetate 30-3 1 1.136 85.29 Xylene 32.5 ... 87.14+
Aniline 30-31 ... very soluble Toluene 25 1.128 83.62
100 gms. pyridine dissolve 381 gms. salol at 2O°-25° (Dehn, 1917). The solu-
tion in aqueous 50 per cent pyridine separates into two layers.
SOLIDIFICATION TEMPERATURES (Solubility, see footnote, p. i) FOR MIXTURES OF:
Salol and Thymol. (Bellucci, 1912.)
Salol and Urethan.
(Bellucci,
1912, 1913.)
AO t Gms. Salol
c r!rf Per I0° Gms.
Sohdif. V Mixture
f o e Gms. Salol
Snlirlif per too Gms.
Solldlf- Mixture.
+o £ Gms. Salol
Solidif per \°° Gms>
Mixture.
t°of
Solidif.
Gms. Salol
Mixture.
42
100
23
So
42
IOO
36.
5
50
34
26
90
80
29
34-5
40
30
36
29
Eutec.
00
86
39
41-5
40
30
18
70
40
20
31
80
44
2O
J3
Eutec.
66
46
10
30
70
47
IO
17
• 5
60
Si
o
3*4
60
48.
5
0
The Eutec
. for sa
lol + cam
phor is at
-1-6° and contains 56%
salol
KBellucci,
The Eutec. for salol 4-monobromcamphorisat2i°and contains 6o%salol. (1912, 13.)
Solidification temperatures for Salol + Sulfonal and for Salol + 0 Naphthol
are given by Bianchini (1914).
SANTONIN CiBHi8O3.
SOLUBILITY IN SEVERAL SOLVENTS.
f. rGmo^ Authorit^
Water 20-25 0.02+ (Dehn, 1917.)
Alcohol (90%) 15 about 2. 3 (Greenish and Smith, 1903.)
Trichlor Ethylene 15 2.46 (Wester and Bruins, 1914.)
Pyridine 20-25 12.72 (Dehn, 1917.)
Aq. 50% Pyridine 20-25 12.35
F.-pt. data for mixtures of stereoisomeric santonin salts are given by Malvino
and Manino (1908).
SAMARIUM CHLORIDE 594
SAMARIUM CHLORIDE SaCl3.
100 gms. pyridine dissolve 6.38 gms. SaCl3 at 15°. (Matignon, 1906, 1909.)
SAMARIUM GLYCOLATE Sa(C2H3O3)?
100 gms. H2O dissolve 0.6373 Sm- Sa(C2h3O3)3 at 20°.
(Jantsch and Griinkraut, 1912-13.)
SAMARIUM Double NITRATES.
SOLUBILITY IN CONC. HNO3 OF dip = 1.325 AT 16°.
(Jantsch, 1912.)
Samarium Magnesium Nitrate [Sa(N03)e]Mg3 . 24 H2O 24 . 55
Nickel " " Ni3 " 29.11
Cobalt " " Co3 " 34.27
Zinc " " Zn3 " 36.47
Manganese " Mn3 " 50.04
SAMARIUM OXALATE Sa2(C2O4)3.ioH2O.
One liter H2O dissolves 0.00054 Sm- Sa2(C2O4)3 at 25°, determined by the
electrolytic Conductivity method. (Rimbach and Schubert, 1909-)
SOLUBILITY OF SAMARIUM OXALATE IN AQUEOUS SOLUTIONS OF SULFURIC ACID
AT 25°.
(Wirth, 1912.)
^THSO^ ^i^Gmf.3 Solid Phase. NA°r^y of °pTr i^Gmf.3 Solid Phase.
Aq.H2S04. *sat. Sol. Aq. H2SO4. »§•*. fc^
I O.IOI5 Sa2(C2O4)3.ioH20 2.8 0.3886 Sa2(C2O4)3.ioH2O
1.445 0.1804 " 4- 32 0.7008
1.93 0.2254 " 6.175 1.072
SAMARIUM Dimethyl PHOSPHATE Sa2[(CH3)2PO4]6.
100 gms. H2O dissolve 35.2 gms. Sa2[(CH3)2PO4]6 at 25° and about 10.8 gms.
at 95°- (Morgan and James, 1914.)
SAMARIUM SULFATE Sa2(SO4)3.
SOLUBILITY IN AQUEOUS SOLUTIONS OF AMMONIUM SULFATE AT 25°.*
(Keyes and James, 1914.)
Clmc rwvr Tfv\ rime TT-O Cirrtc r\**r T/V\ Clmc TT_O
Solid Phase.
+(NH4)2SO4
(NH4)2S04.
Sa2(S04)3.
ouiiu .rjiase.
(NH4)2S04.
Sa2(S04)3.
0.03
2.1
802(8003
32.5
0.9
0.8
2
"
46.3
I
i .1
2.8
" +1.1.7
77-5
i-3
1.9
i-5
1.1.7
77-3
o-3
7-4
0.8
«
76.8
0.6
18.8
0.8
«
1.1.7 =Sa2(S04)3.(NH4)2S04.7H20.
SOLUBILITY IN AQUEOUS SOLUTIONS OF SODIUM SULFATE AT 25°.*
(Keyes and James, 1914.)
Gms. per too Gms. H2O. Gms. per 100 Gms. H2O.
•N^SO.. •sa.CSO.)..' SO"dPhaSe- ' Na,SO.. ' Sa,(SO.).; "•
2 . 05 Sa2(SO4), 10.51 0.012 2Sa2(SO4)3.3Na2SO4.6H2O
O.I 2 " 14.71 0.010
0.5 O.I I 2Sa2(S04),.3Na2SO4.6H2O 2O.O2 O.OI2
1.9 0.03 " 23.68 0.018 "
6.44 0.016 " 27.40 o.on "
* The mixtures were rotated at constant temperature for 5 months.
loo cc. anhydrous hydrazine dissolve I gm. Sa2(SO4)3 at room temp.
(Welsh and Broderson, 1915.)
595 SAMARIUM SULFONATES
SAMARIUM SULFONATES
SOLUBILITY IN WATER.
Gm. An-
Salt. Formula. t°. J^^G^1 Authority.
H20.
Samarium m Nitro-
benzene Sulfonate SatCjILXNO^SOskyHzO 15 50.9 (Holmberg, 1907.)
Samarium Bromonitro-
benzene Sulphonate Sa[C6H3(i)Br(4)N02(2)SO3]3.ioH2O 25 7.84 (Katz and James, 1913.)
SCANDIUM OXALATE Sc2(C2O4)3.5H2O.
SOLUBILITY IN AQUEOUS SOLUTIONS OF AMMONIUM OXALATE AND OF HYDRO-
CHLORIC ACID.
In Aq. Ammonia Oxalate at 25°. In Aq. Hydrochloric Acid at 25°
(Wirth, 1914.) , and at 50°. (Meyer, 1914.)
Gms. per 100 Gms. Gms. Sc2(C2O4)3 per
Sat. Sol. Solid Phase. NoArmsi1& o£ 100 Gms. Sat. Sol.
-QOa" Sc203. 'Atas0. At SoV
1.624 0.3019 Sc2(C2O4)s SH2O O.I 0.0299 0.0420
2.4 O.40I2 " 0.5 0.0650 0.0870
4.478 0.7108 " +(NH4)2C2O4 I O.IO20 O.I435
2 0.1716 0.2556
5 0.4170 0.6533
SOLUBILITY IN AQUEOUS SOLUTIONS OF SULFURIC ACID.
Results at 25°. (Wirth, 1914.) Results at 25° and at 50°. (Meyer, 1914.)
Normality of
Aq. H2SO4.
per zoo Gms.
Sat. Sol.
Solid Phase. N«ngjgjof
Gms. Sc2(C
'2O4)3 per 100 Gms.
Sat. Sol.
At 25°.
At 50°.
I
0.1148
Sc,(CA)a.5H*) O.I
0.0385
0.0562
2.1
0.2573
0-5
0.0997
0.1481
2-43
0.2904
I
0.1663
0.2493
3-57
0.4204
2
0.3176
0.4429
4.86
0.5834
5
0.7761
I.I280
100 gms. sat. solution of scandium oxalate in 2.43 n H2SO4 + 0.5 n oxalic
acid contain 0.0284 gm- Sc2O3 at 25°. (Wirth, 1914.)
SCANDIUM SULFATE Sc2(SO4)3.5H2O.
SOLUBILITY IN WATER AND IN AQUEOUS SULFURIC ACID AT 25°. (Wirth, 1914.)
Gms. Sc2(SO4)3 Gms. Sc2(SO4>3
Solvent. per 100 Gms. Solid Phase. Solvent. per 100 Gms. Solid Phase.
Sat. Sol. Sat. Sol.
Water 28.52 Sc2(SO4)3.sH2o 4.86wH2S04 8.363 Sc2(SO4)3.sH2o
o.5wH2S04 29.29 " 9.73ttH2SO4 1.315
i wH2SO4 19.87 22.35nH2SO4 0.484 Sc^SO^.sHzO
Scandium sulfuric acid double sulfate, Sc2(SO4)3.3H2SO4. 100 gms. sat. sol. in
cone. H2SO4 of d = 1.6 contain 0.8616 gm. of the double salt. (Wirth, 1914.)
SEBACIC ACID (CH2)8(COOH)2.
100 gms. 95% formic acid dissolve 1.05 gm. sebacic acid at 19°. (Aschan, 1913.)
DISTRIBUTION OF SEBACIC ACID BETWEEN WATER AND ETHER AT 25°.
(Chandler, 1908.)
Mol. Concentration of Sebacic Acid in:
Ratio.
Aq. Layer. Ether Layer.
O.00062 O.O29I O.O2I3
O.OOO58 O.O272 O.O2I3
0.00047 0.0213 0.0221
0.00036 0.0155 0.0232
SELENIUM 596
SELENIUM Se.
SOLUBILITY IN CARBON BISULFIDE.
(Marc, 1906.)
100 cc. CSj dissolve 0.065 gm. amorphous Se at room temperature. Se which
is heated to 180° for 6-7 hours is insoluble in CSa. Se crystallized from the
melt at 200° is insoluble in CS-j. Se heated once quickly to 140° is very slightly
soluble in CSa.
100 cc. CSz dissolve at the boiling-point 3-3.4 mgs. Se which has been heated to
140° for i hr.
100 cc. CSj dissolve at the boiling-point 2 mgs. Se which has been heated to
195° for 2 days. (Marc, 1907.)
,100 gms. methylene iodide (CH2I2) dissolve 1.3 gms. Se at 12°. (Retgers, 1893.)
SOLUBILITY OF Mix CRYSTALS OF SELENIUM AND SULFUR IN CARBON DISULFIDE
AT 25°. (Ringer, 1902.)
Mols. per 100 Mols. Solution. Mol.Per Mols. per 100 Mols. Solution. Mol. Per
,— - — - *- - — - Cent Se in /-— - -* - - - . Cent Se in
CSj. Se. S. Crystals. CS2- Se- S. Crystals.
43-i o . 56.9 o 58.24 2.35 39.41 55.67
45-i o-93 53-97 3-54 64.66 1.58 33.76 68.38
44.98 1.03 53.99 3.81 8r.ii 2.4 16.49 58.7
47.84 2.07 50.59 8.69 88.41 2.17 9.42 61.5
49.54 2.19 48.27 16.4* 91-38 1.68 6.94 65
47.62 2.16 50.22 14.2* 99-51 °-49 o ioof
46.12 1.485 52.39 29-35* 99-14 0.86 o iooj
* Mix crystals homogeneous in all except these solutions.
t = Solubility of hexagonal selenium. t = Solubility of amorphous selenium.
Fusion-point curves for mixtures of selenium and other metals are given by
Pelabon (1909). Results for Se + Te are given by Pellini and Vio (1906).
Diohenyl SELENIUM BROMIDE (C6H6)2SeBr2.
"RECIPROCAL SOLUBILITY OF DIPHENYL SELENIUM BROMIDE AND DIPHENYL
TELLURIUM BROMIDE IN WATER AT 25°.
(Pellini, igo6a.)
Gms. per 1000 cc. Sat. SoL Mo1- % (C6H6)r Qms. per 1000 cc. Sat. Sol. Mol.
'(C,H6)2TeBr2. * (C6H5)2SeBr2.' bC Mixture^' (QH^TeBr,. " (C6H5)2SeBr2. *
18.614 ° o 10.224 14.608 44-89
17.400 1.448 4.91 7.544 19.876 51.18
16.152 4-172 10.51 6.780 18.984 94-25
15.030 6.210 18.21 3-184 17.392 95-82
13.320 8.148 24.98 o 18.984 100
11.940 11.420 34-94
SELENIC ACID H2SeO4
SOLUBILITY IN WATER, DETERMINED BY FREEZING-POINT METHOD.
(Kremann and Hofmeier, 1908.)
Gms. H2SeO4 Gms. H2SeO4
t°. per 100 Gms. Solid Phase. t°. per 100 Gms. Solid Phase.
Sat. Sol. Sat. Sol.
o o Ice — 55 71.5 H2SeO4.4H2O
— 10 21
— 20 •. 30
-30 36
—40 40
-50 42.5
—65 Eutec. 74 " +H2SeO4.H,0
— 50 75.5
-20 79
o 81
+20 85
—60 45 26 m. pt. 88
—80 48 ' " 20 91 "
-95 Eutec. 50 « +HzSe04.4H20 16 Eutec. 91.5 " +HfSeO4
-80 52 H2Se04.4H20 30 93 H2Se04
-70 54 " 40 94.5
-60 58 " 50 96.5
— 51 m. pt. 67 " 60 loo "
597
SELENIOUS ACID
SELENIOUS ACID
H2SeO3.
SOLUBILITY IN WATER.
(Etard, 1894.)
— IO
O
+ 10
20
Cms. H2SeO3 per
100 Cms. Solution.
42.2
47-4
55
62.5
25
30
40
50
Cms. H2SeO3 per
100 Cms. Solution.
67
70.2
77-5
79.2
60
70
80
90
Cms. H2SeO3 per
100 Cms. Solution.
79-3
79-3
79-3
79-4
SELENIOUS ANHYDRIDE (Selenium Dioxide) SeO2.
SOLUBILITY IN SEVERAL SOLVENTS.
(de Coninck, 1906.)
Solvent.
Water
Ethyl Alcohol (93%)
Methyl Alcohol
Acetone
Acetic Acid (Glacial)
SILICA Si02.
SOLUBILITY IN WATER AND IN AQUEOUS SOLUTIONS OF ACIDS.
(Lenher and Merrill, 1917.) .
A platinum bottle and stirrer were used. The silica was prepared by adding
silicon tetrachloride to water. The gel thus formed was washed until free of
HC1 and dried between filter papers. Conductivity water was used and equi-
librium was reached within 24 hours. The saturated solution was evaporated
to dryness in a platinum dish. The residue was weighed and the silica volatil-
ized with HF1 + H2SO4. The difference was considered to show "the amount
of silica which had changed from an unfiiterable to a filterable state of division."
t°.
11-3-15
Cms. SeO2 per
100 cc. Solvent.
38.5
14.1
ii. 8
10.2
6.66
15-3
4-35
12.9
i. ii
At
25°.
Per cent
HC1.
0
Gm. SiO2 per
50 cc. Sol.
O.OOSo
3
6-3
0.00665
o . 00465
II. I
18.9
25.1
34-6
0.00245
0.0008
O.OOO6
0.0003
Results for Aq. HC1:
At 90°.
Results for Aq. H2SO4:
At 90°.
Per cent
HC1.
O
2
3
5-4
7.6
10
13.6
18.6
Gm. SiO2 per
50 cc. Sol.
0.0213
0.0198
0.0186
0.0152
0.0115
0.0091
0.0056
0.0029
Per cent
H2S04.
Gm. SiO2 per
50 cc. Sol.
3-9
0.02II
7-3
0.0186
15.6
O.OII2
25.4
0.0058
36
0.0034
46.9
0.0013
55.6
O.OOO5
71
0.0004
At 90°, a slow current of CO2 through the solutions did not affect the results.
Ignited silica reaches equilibrium very slowly as compared with silica gel. The
true solubility of ignited silica is probably the same as that of gelatinous silica.
SOLUBILITY OF SILICA IN MELTED CALCIUM CHLORIDE.
(Arndt and Lowenstein, 1909.)
800
850
900
950
Cms. SiO2
per 100 Gms.
Sat. Solution.
2-5
3-8
5-4
7.6
SILICON Si 598
SOLUBILITY IN LEAD, IN ZINC AND IN SILVER.
(Moissan and Siemens, 1904.)
In Lead. In Zinc. In Silver.
j.o Gm. Si per ^ 0 Gm. Si per ^ 0 Gm. Si per ioo Gms.
ioo Gms Lead. ioo Gms. Zinc. Silver.
1250 0.024 600 0.06 970 9.22(58.02)
1330 O.O7O 650 O.I5 H5O 14.89(27.66)
1400 0.150 730 0.57 1250 19.26 (19)
1450 0.210 800 0.92 1470 41.46(16)
1550 0.780 850 1.62
The silicon which crystallized from the saturated solution in silver was found
to be incompletely soluble in HF. The figures in parentheses show the per-
centage soluble in HF in each case.
Freezing-point data for mixtures of silicon tetraphenyl and tin tetraphenyl
are given by Pascal (1912).
SILICON IODIDES Si2I6, SiI4.
SOLUBILITY IN CARBON DISULFIDE.
(Friedel and Lachburg, 1869; Friedel, 1869.)
IOO gms. CSa dissolve 19 gms. Si2Ie at 19°.
IOO gms. CSa dissolve 26 gms. Si2I6 at 27°.
ioo gms. CSa dissolve 2.2 gms. SiI4 at 27°.
SILICO TUNGSTIC ACID H8SiWi2O42.
ioo gms. H2O dissolve 961.5 crystallized silico tungstic acid at 18°, and the
solution has Sp. Gr. 2.843.
SILVER Ag.
For equilibrium between metallic Silver and mercury (Silver amalgam) and
mixed aqueous solutions of their nitrates, determined for mixtures of the two
metals in all proportions, see Reinders, 1906.
SILVER ACETATE CH3COOAg.
SOLUBILITY IN WATER.
(Nernst, 1889; Arrhenius, 1893; Goldschmidt, 1898; Nauman and Rucker, 1905; Raupenstrauch,
1885; Wright and Thompson, 1884, 1885.)
to Gms.Ag(C2H3O2) to Gms. Ag(C2H3O2) te Gms. Ag(C2H3O2)
per Liter. per Liter. per Liter.
O 7-22 25 II. 2 50 16.4
IO 8.75 30 12. I 00 18.9
15 9.4 40 14- r 7° 2I-8
20 10.4 80 25.2
SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF:
Silver Nitrate. Sodium Acetate.
Gms. CH3COOAg per Liter at: rnJrOON Gms- CH3COOHg per Liter at:
pergLiter. 16° (Nernst). 'i9.8°(Arrhenius). per Liter * '16° (N.,N.andR.). i8.6°(A.). '
o 10.05 9-^5 o 10.05 9-9
5 8.2 7.9 5 6.3 6.6
10 7 .o 6.6 10 4.6 4.9
15 6-4 5-5 J5 3-8 4-i
20 5.7 4-5 20 3-3 3-5
30 4.4 ... 30 ... 2.8
40 3.2 ... 40 ... 2.4
599 SILVER ACETATE
SOLUBILITY OF SILVER ACETATE IN AQUEOUS SALT SOLUTIONS AT 25°. (jaques, 1910.)
Aq. Solution of;
Water alone
Cadmium Acetate
ii ii
Lead Acetate
o
ii. 08
i-i5
10.39
5.76
8.10
11.52
6.71
57-6
4-33
115.2
3-95
1.63
10.69
8.13
9-45
16.26
8-34
81.3
7.26
162.6
5-99
Aq. Solution of:
Potassium Acetate
Silver Nitrate
Sodium Acetate
Gms. Salt
per Liter.
2.22
Gms.
AgCjHA
per Liter.
9.60
22.2
4-43
III
222
2.41
2.18
2.77
9-93
5-55
9
II. 10
22.21
7.41
5-8i
1.97
9.27
19.7
98.5
4.21
2-33
197
2.07
SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT 25°.
(Hill and Simmons, 1909.)
Normality of
Aq. HNO3.
Per cent HNO3 in
Solvent. S
4* of
at. Sol.
Gms. AgQHsOj
per Liter Sat. Sol.
0
0 ]
[.005
11.13
0.50
3.096 ]
[.072
85-3I
I
6.128 ]
.I4O
161.9
2
11.757 -a
.267
307-4
4.02
22.386 3
.470
549-3
5-03
27.328
.561
656
6.44
r _ -u_ _-i-.t-Mr.i- t A _./•
.670
792.2
Results are also given for the solubility of AgC2H3O2+AgNO3 in Aq. HNO3at 25°.
SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF SEVERAL
COMPOUNDS AT 25°. (Armstrong and Eyre, 1913.)
Gms.
Gms.
Aqueous
Solution of:
wuiiipouuu
per
1000 Gms.
rtg^2n3^f2
per 1000
Gms.
Aqueous
Solution of:
H20.
Sat. Sol.
0
II. 08
Propyl Alcohol
II
10.13
II
8.92
Glycerol
33
9.16
Glycol
66.4
7-55
u
Water
Acetaldehyde
Paraldehyde
ii
Isobutyl Alcohol
SILVER MonochlorACETATE CH2ClCOOAg.
One liter aqueous solution contains 12.97 gms. CHjClCOOAgat 16.9°. (Arrhenius/93.)
Gms.
Gms.
Compound
per
looo Gms.
per 1000
Gms.
H20.
Sat. Sol.
15
9.88
60
8.03
9.21
8.66
15-5
10.86
62.1
8.44
SOLUBILITY OF SILVER MONO CHLOR ACETATE AT 16.9
AQUEOUS SOLUTIONS OF:
IN
Silver Nitrate.
Sodium Chlor Acetate.
Gms.
AgNOa
per Liter.
Gms.
CH2ClCOOAg
per Liter.
Gms.
CH2ClCOONa
per Liter.
Gms.
CH2ClCOOAg
per Liter.
0-0
9.6
17.0
12-97
10.05
7-55
O-O
3.88
7-77
15-53
12.97
10.05
8.16
6. 02
31.07
58.26
4.19
3.26
SILVER ACETATE
600
SOLUBILITY OF SILVER MONOCHLORO ACETATE IN NITRIC ACID AT 25°.
(Hill and Simmons, 1909.)
Normality
Gms. HN03
Gms.
of Aq.
HN03.
per 100 Gms.
Solvent.
Sa* Sol.
AgC2H2C102
per Liter.
0
0
.0095
I5.I8
0.25
1.564
.0426
50.33
0.50
3.096
.0791
91.83
I
6.128
•1473
167.3
2
n-757
.2716
310.8
4
22.277
•4749
549-1
5
27.185
•5673
659.2
SILVER Dipropyl ACETATE AgC8H15O2.
100 gms. H2O dissolve 0.123 gm. AgC8Hi502 at 11.7°, and 0.190 gm. at 72°.
(Fiirth, 1888.)
SILVER Methyl Ethyl ACETATE Ag.CH3.CH2CH(CH3)COO.
SILVER Diethyl ACETATE Ag[(C2H5)2CH.COO].
SILVER Trimethyl ACETATE Ag(CH3)3CCOO.*
SOLUBILITY OF EACH IN WATER.
(Sedlitzky, 1887; Keppish, 1888; Stiassny, 1891.)
Gms. per 100 Gms. H2O.
Gms. per 100 Gms. H2O.
I .
Ag.C5H902.
AgC.HuOj.
AgC5H902.*
i .
AgCBH902.
AgC.HuO,.
AgC5H902.*
0
I .112
0.402
1. 10
50
I. 602
0-536
i-47
10
I .126
0.413
I-I5
60
1.827
0.585
i-57
20
I.I82
0.432
1.22
70
2.093
0.643
1.68
30
1.280
0.458
1.22
80
2.402
i. 80
40
I .420
0.494
1-37
SILVER ARSENATE Ag3AsO4.
One liter H2O dissolves 0.0085 gm.Ag3AsO4 at 20°. See Note, p. 608. (Whitby, 1910.)
SILVER ARSENITE Ag3AsO3.
One liter H2O dissolves o.oi 15 gm. Ag3AsO3at 20°. See Note, p. 608. (Whitby, 1910.)
SILVER BENZOATE C6H6COOAg.
One liter of aqueous solution contains 1.763 gms. C6H5COOAg at 14.5°, and 2.607
gms. at 25°. (Holleman, 1893; Noyes and Schwartz, 1898.)
SOLUBILITY OF SILVER BENZOATE AT 25° IN AQUEOUS SOLUTIONS OF:
Gms. per Liter.
Nitric Acid (N. and S.).
Gms. Mols. per Liter. Gms. per Liter.
Chloracetic Aci<
Gms. Mols. per Liter.
HNO3.
COOAg.
HNO3.
C«H6
COOAg.
C1COOH.
C6H5
COOAg.
0
0
.01144
O
2 .607
O
0
.01144
0
-004435
0
•01395
O
.280
3-195
o
.00394
0
.01385
0
.00887
O
.01698
O
•559
3.889
0
,00787
O
.Ol6l2
O
.00892
0
.01715
O
.562
3.926
o,
01574
0
.02093
O
.01774
0
.02324
X
.118
5-321
O
.02674
0
.03071
I
.686
7.031
CH2
C6H6
C1COOH. COOA5g.
o 2.607
0.371 3.172
0.744 3.691
1.487 4.792
One liter of cold alcohol dissolves 0.169 gm. C6H6COOAg; one liter of boiling
alcohol dissolves 0.465 gm. (Liebermann, 1902.)
SILVER BORATE AgBO2.
One liter of aqueous solution contains about 9.05 gms. AgBO2 at 25°.
(Abegg and Cox, 1903.)
Normality of Aq.
Acetic Acid.
o . 0498
0.0997
0.1995
Gms. AgBrO3 per
Liter.
1.9429
1-9379
1.9206
Normality of Aq.
Acetic Acid.
0.4988
0-9975
1.8721
6oi SILVER BROMATE
SILVER BROMATE AgBrO3.
SOLUBILITY IN WATER.
t°. Cms. AgBrO3 per Liter. Authority.
20 I . 586 (BSttger, 1903.)
24.5 I.gil (Noyes, 1900.)
25 1.68 (Longi, 1883.)
27 I . 71 (Whitby, 1910, see note, p. 608.)
25 1-949 (Hill, 1917.)
SOLUBILITY OF SILVER BROMATE IN AQUEOUS ACETIC ACID AT 25°.
(Hill, 1917-)
Cms. AgBrO3 per
Liter.
1.863
I.80I3
1.6178
SOLUBILITY OF SILVER BROMATE IN AQUEOUS AMMONIA AND NITRIC
ACID SOLUTIONS AT 25°.
(Longi, 1883.)
Gms. AgBrO3 per
Solvent. , -T-5 i±I _,
1000 cc. Sol. 1000 Gms. Sol.
Ammonia Sp. Gr. 0.998 = 5% 35.10 35.54
Ammonia Sp. Gr. 0.96 = 10% 443.6 462.5
Nitric Acid Sp. Gr. 1.21 =35% 3.81 3.12
SOLUBILITY OF SILVER BROMATE AT 24.5° IN AQUEOUS
SOLUTIONS OF:
Silver Nitrate (Noyes). Potassium Bromate (N.).
Normal ^Content. Gms. per Liter. Normal Content. Gms. per Liter.
AgN03. AgBr03." 'AgNOs- AgBrO3. KBrO3. AgBrO3". KBrO3. AgBrOi
o.o 0-0081 o.o 1.911 o.o 0.0081 o.o 1.911
0.0085 0.0051 1-445 I-203 0.0085 0.00519 1-42 1-225
0.0346 0.0022 5.882 0.510 0.0346 0.00227 5.78 0.536
SILVER BROMIDE AgBr.
SOLUBILITY IN WATER.
t °. Gms. AgBr per Liter. Authority.
2O O -000084 (Bottger — Z. physik. Ch. 46, 602, '03.)
25 O .OOOI37 (Abegg and Cox — Z. physik. Ch. 46, u, '03.*
IOO O • OO3 70 (Bottger — Z. physik. Ch. 56, 93, '06.)
(See alsoHolleman — Z. physik. Ch. 12, 129, '93; Kohlrausch — Ibid. 50, 365, '05.)
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS AMMONIA SOLUTIONS.
(Longi — Gazz. chim. ital. 13, 87, '83; at 80°, Pohl — Sitzber. Akad. Wiss. Wien, 41, 267, '60.)
Gms. AgBr at 12° per Gms. AgBr at 80° pet
Solvent. 1000 cc. 1000 Gms. IO°°1 Gms-
Solvent. Solvent. Solvent.
Ammonia Sp. Gr. 0.998=5% 0.114 0.114 ...
Ammonia Sp. Gr. 0.96 =10% 3-33-4-0 3.47
Ammonia Sp. Gr. 0.986 ... 0.51*1.0!
* Dried AgBr. t Freshly pptd.
SILVER BROMIDE
602
SOLUBILITY OF SILVER
Results at 15°.
(Bodlander, 1892.)
BROMIDE IN AQUEOUS AMMONIA SOLUTIONS.
Results at 25°. Results at 25°.
(Bodlander and Fittig, 1901-02.) (Whitney and Melcher, 1903.)
<*lfi.5 Of
Sat. Sol.
Cms. Mols. per Liter. Gms. Mols. per roc
o Gms. H2O.
G
oncentrat
ion
per Liter.
'NH3.
Ag2Br2.
NH3.
AgBr.
G. Mols. NH3.
G
. Atoms Ag.
0.9932
1.085
0
.0011
0
.1932
0
.OOO6O
0
.0764
0
.000276
0-9853
2.365
o
.0031
o
.3849
o
.00120
0
•115
O
.000391
0.9793
3.410
0
.0050
0
•7573
0
.00223
0
.268
O
.000941
O.972O
4-590
0
.0074
I
•965
0
.00692
o
•273
0
.00107
O-Q^SS
5-725
0
.OIOI
3
.024
o
.01163
o
•450
0
.00170
5.244 0.02443 0.497 0.00159
SOLUBILITY OF SILVER BROMIDE IN
Ammonia at o°.
(Jarry, 1899.)
Grams per TOO cc. Solution.
AQUEOUS SOLUTIONS OF:
Monomethyl Amine at 11.5°.
(Jarry.)
Gms. per 100 cc. Solution.
NHsGas.
AgBr.
NH3 Gas.
AgBr.
3-07
O.oSo
26.27
1.067
4.88
0-096
31.26
1.568
6.69
O.I72
33-89
I.987
8.29
0.212
36-52
2 .669
11.51
c-349
37-22
2.888
I5-32
o-557
37-70
2.930
18.09
0.722
39.26
2.892
19-53
0.741
39-95
2.852
NH2CH3.
AgBr.
II .01
O.O7
13 . 17
O.I2
J5 •I3
0.16
17.97
32-58
35-62
0.28
o-55
o-73
43 •"
48.44
1.27
2.89
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF METHYL
AMINE AND OF ETHYL AMINE AT 25°.
(Bodlander and Eberlein, 1903; Wuth, 1902.)
In Methyl Amine. In Ethyl Amine.
Mols. per Liter. Mols. per Liter.
Total Base. AgBr. Free Base.*
1.017 0.0025 i. 012 (B.&E.)
0.508 0.0013 0.505 (B.&E.) 0.200
0.203 0.00049 0.202 (B.&E., W.) o.ioo
0.102 0.00026 o.io2(B.&E.) 0.103
0.00026 o.io2(B.&E.)
0.0947 0.00041 ... (W.)
0.051 0.00012 0.051 (B.&E.)
0.04 0.00034 ... (W.)
O.O2 O.OOO26 ... (W.)
Total Base. AgBr. Free Base.*
0.483 0.00231 0.478 (B.&E.)
0.00097 0.198 "
0.000475 0.099 "
0.000711 . . . (W.)
0.06572 0.000258 ... "
0.05512 0.000193 • • • "
0.03942 0.000137 • • • "
0.01272 0.0000867
* The free base is found by subtracting from the total base two mols. of base for each atom of dissolved Ag.
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF MERCURIC
NITRATE AT 25°.
(Morse, 1902.)
Mols. HgNOr Mols. AgBr Gms. AgBr
(HNOs) per Liter. per Liter. per Liter.
I 0.03660 6.878
o.io 0.00873 1.640
o . 05 o . 0063.9 T • 2O°
Since HNO3 was present in all cases, its influence on the solubility was ex-
amined. It was found that no appreciable differences were obtained with con-
centrations varying between o.i and 2 normal HNOa. Both crystallized and
amorphous silver bromide gave identical results.
Mols. HgNOr
(HN03) per Liter.
0.025
O.OI25
O.OIOO
Mols. AgBr
per Liter.
0.00459
0.00329
o . 00306
Gms. AgBr
per Liter.
0.863
0.618
0-575
603 SILVER BROMIDE
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SALT SOLUTIONS.
(Mees and Piper, 1912.)
Aqueous Solution. t°. Gms. AgBr
per Liter.
Aq. i per cent Sodium Thiosulf ate ? 2 . 06
" Ammonium Thiocyanate 0.03
" " Ammonium Carbonate " 0.004
" " Sodium Sulfate " 0.055
" " Thiocarbamide " 1.49
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SALT SOLUTIONS.
(Valenta, 1894; see also Cohn, 1895.)
Gms.AgBr per 100 Gms.Aq. Solution of Concentration:
Salt Solution. t°. / * >
1:100. 5:100. 10: 100. 15:100. 20:100.
Sodium Thio Sulphate 20 0.35 1.90 3.50 4.20 5.80
" " Calc. by Cohn 20 0.50 2.40 4.59 6.58 8.40
Sodium Sulphite 25 ... ... 0.04 ... 0.08
Potassium Cyanide 25 ... 6.55
" Calc. by Cohn 25 ... 6.85
Potassium Sulphocyanide 25 0.73
Ammonium Sulphocyanide 20 ... 0.21 2.04 5-30
Calcium Sulphocyanide 25 0.53
Barium Sulphocyanide 25 0.35
Aluminum Sulphocyanide 25 ... ... 4.50
Thio Carbamide 25 1.87
Thio Cyanime 25 0.08 0.35 0.72
NOTE. — Cohn shows that the lower results obtained by Valenta are due to the
excess of solid AgBr used and the consequent formation of the less soluble di salt,
3(AgS2O3Na)2, instead of the more soluble tri salt, (AgS^OsNa^NazSzOs.
100 cc. H2O containing 10 per cent of normal mercuric acetate, Hg(C2H3O2)2-h
Aq.f dissolve 0.0122 gm. AgBr at 20°.
100 gms. NaCl in cone. aq. solution dissolve 0.474 g™- AgBr at 15°.
100 gms. NaCl in 21 per cent solution dissolve 0.182 gm. AgBr at 15°.
100 gms. KBr in cone, solution dissolve 3.019 gms. AgBr at 15°.
95 gms. NaCl + 10 gms. KBr in cone. aq. solution dissolve 0.075 gm. AgBr
at 15°. (Schierholz, 1890.)
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS POTASSIUM BROMIDE AT 25°.
(Hellwig, 1900.)
Mols. KBr per Liter 2.76 3.68 4.18 4.44 4.864
Gms. KBr per Liter 2.20 7.50 13.50 17 .95 26.44
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF SODIUM SULFITE.
Results at Room Temperature (?). Results at 25°.
(Mees and Piper, 1912.) (Luther and Leubner, i9i2a.)
Gms.
per Liter.
Gms. per Liter.
Gms. Formula Weights
per Liter.
Na2SO3.
0.08
0.17
0.30
o-59
1-13
2.08
AgBr.
o . 000746
O . OO2 19
0.00393
o . 00448
O.OO865
0.01585
Na^Oa.
4.85
9-47
I7-65
3^.2
70.75
83.75
AgBr.
0.0329
0.05264
0.116
0.265
0-57
0.79
S03".
0.232
0.406
0.448
0.466
0-474
0.675
Ag'.
O.OO25
0.0023
0.0023
0.0053
0.0055
0.0084
SILVER BROMIDE
604
SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF SODIUM
THIOSULFATE AT 35°.
(Richards and Faber, 1899.)
Cms. Cryst. Na
Thiosulfate
per Liter.
Cms. AgBr
Dissolved per Gm.
of Thiosulphate.
Mols. AgBr
Dissolved per
Mol. of Na«SA.
100
0.376
0.496
2OO
0.390
0-SI5
300
400
o-397
0.427
, 0.524
0.564
100 cc. of 3 n AgNO3 solution dissolve 0.04 gm. AgBr at 25°. (Hellwig, 1900.)
Fusion-point data for mixtures of AgBr + AgCl and AgBr + Agl are given by
Monkemeyer -(1906). Results for AgBr + NaBr are given by Sandonnini and
Scarpa (1913)-
SILVER BUTYRATE C3H7COOAg.
SILVER (Iso)BUTYRATE (CH3)2CHCOOAg.
SOLUBILITY OF EACH SEPARATELY IN WATER.
(Goldschmidt, 1898; Arrhenius, 1893; Raupenstrauch, 1885.)
Cms. per too Gms. H2O.
Cms. per 100 Gms. H2O.
I . f— —
Butyrate.
— — > I/ .
Iso Butyrate.
Butyrate.
Iso Butyrate.
O
O
.363
0.796
30
0.
561
I
.060
(l.I022)
10
O
.419
0.874
40
O.
647
I
.176
(R.)
I7.8
0
.432
(A.)
50
O.
742
I
.313
18.8
0
-445
(A.)
60
O.
848
20
O
.484
0.961
(0.9986)
70
0.
964
I
.670
25
.
(1.0442)
80
I .
14
I
.898
SOLUBILITY OF SILVER BUTYRATE IN AQ. SOLUTIONS OF SILVER ACETATE,
SILVER NITRATE AND OF SODIUM BUTYRATE.
(Arrhenius, 1893.)
In Silver Acetate at 17.8°. In Silver Nitrate at 18.8°.
G. Mols,
, per Liter.
Grams per Liter.
G. Mols^per Liter.
Grams per Liter.
COOAg.
C3H7
COOAg.
' CH3
COOAg.
C3H7
COOAg.
AgNO3.
C3H/
COOAg.
AgNOa-
COOAg.
0.0
O-O22I
o.o
4-32
o.o
O.O228
o.o
4-445
0.0270
0.0139
4-51
2.71
0.0667
0.0078
n-33
1.521
0.0506
O.OIO3
8-45
2 -OI
O.IOO
O.OO62
17.00
1.209
G. Mols. per Liter.
COONa. COOAg.
o.o 0.0224
O.OO66 O.OI99
0.0164 0.0169
0-0329 O.OI3I
In Sodium Butyrate at 18.2°.
Grams per Liter.
COONa. COOAg
0-0 4-363
0.73 3-881
1.81 3.296
3-62 2.555
G. Mols. per Liter.
' C3H7 C3H7 '
COONa. COOAg.
0-0658 O.OO9I
0.1315 0-0060
0.263 O.OO4O
0.493 O-OO27
Grams per Liter.
C3Hr
COONa.
7-24
14-47
COOAg.
1-774
.170
28.96 0.780
54.28 0.526
605 SILVER CAPROATES
SILVER CAPROATES Ag(C6HnO2).
SOLUBILITY OF EACH SEPARATELY IN WATER.
(Keppish, 1888; Stiassny, 1891; Kulisch, 1893; Konig, 1894; Altschul, 1896.)
Results in terms of gms. salt per 100 gms. H2O.
a Methyl Pentan
Methyl 3 Pentan 4 Methyl Pentan
Normal Caproate 4 Acid
Acid 4 4 Acid
»«.
CH3(CH2)4COOAg. CH3.CH.CHa
CH3.CH2 CH3(CH2)2CH(CH3)
.CHCH3CH2COOAg. .COOAg.
.(CH2)2COOAg.
o
0.076 (A.) 0-078(Keppish) O.l68 (Konig) o .880 (Kulish) o .510 (Stiassny)
10
0-085 0.089 O.l62
0.858 0.528
20
o.ioo 0.107 0.163
0.849 °-55°
3°
O..I23 0.131 0.170,
0.854 0.574
40
0.154 0.161 0.183
0.871 0.602
5°
0.193 0.198 0.203
0.902 0.632
60
0.240 0.243 0.229
o . 946 o . 666
7o
0.295 0-288 0.263
i . 003 o . 702
80
0-354 0.300
1.073 °-742
90
0-347
1.157
SILVER CARBONATE Ag2CO3.
SOLUBILITY IN WATER.
t°. Gms. Ag2CO3 per Liter.
Authority.
15 0.031
(Kremers, 1852.)
25 0 . 033 (0.00012 gm. atoms Ag.)
(Abegg and Cox, 1903.)
25 0.032 (by potential measurement) (Spencer and Le Pla, 1909.)
loo 0.50
(Joulin, 1873.)
15 0.85 (in H2O sat. with COz)
(Johnson, 1886.)
SILVER CHLORATE AgClO3.
100 gms. cold water dissolve 10 gms. AgClO3 (Vauquelin); 20 gms. AgC103
(Wachter).
SILVER CHLORIDE AgCl.
SOLUBILITY IN WATER.
(A large number of determinations are quoted by Abegg and Cox, 1903; see also Kohlrausch, 1904- 05;
Bottger, 1903, 1906.)
t°. 14°. 20°. 25°. 42°. 100°.
Gms. AgCl per Liter 0.0014 0.0016 0.0020 0.0040 0.0218
More recent determinations are as follows:
**• Gw'uf£l Method' Authority.
10 0 . 00089 Conductivity (Kohlrausch, 1908.)
l8 O.OOI5O Conductivity (Melcher, 1910.)
21 O . OOI 54 Colorimetric (See Note, p. 608) (Whitby, 1910.)
25 0.00172 Analytical (Glowczynski, 1914.)
5O 0.00523 Conductivity (Melcher, 1910.)
IOO O.O2IO7 (Melcher, 1910.)
loo 0.0217 Colorimetric (Whitby, 1910.)
Note in the case of determination by Glowczynski, one liter of sat. solution was treated with freshly dis-
tilled ammonia and evaporated to dryness in a platinum dish. The residue was dissolved in strong am-
monia and again evaporated. The residue then dissolved in 5-6 cc. of 0.05 n KCN and the silver separated
electrolytically, dissolved in HNO3 and titrated with o.oi n NH<SCN.
Comparative determinations of the solubilities of AgCl, AgSCN, AgBr and Agl
in water at 25°, showed that if the solubility of AgCl be taken as I, that of AgSCN
is 0.0748, that of AgBr is 0.0550 and that of Agl is 0.00077. (Hill, 1908.)
SILVER CHLORIDE
606
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS AMMONIA SOLUTIONS AT 25°.
(Whitney and Melcher, 1903.)
Gm. Mols.
Gm. Atoms
NH, (total)
per Liter.
Ag
per Liter.
0.0282
O.OCI4I
0.0288
O.OOI49
0.0590
o . 00304
O.II8
0.00621
0-253
O.OI4O
o-397
0.0227
0.428
O.O249
0.818
0.0514
0.863
0.0541
0.896
0.0569
0.909
0.0584
0.961
0.0616
1.991
0.147
2.042
0.151
(Straub, 1911.)
Gm. Mols.
Gm. Atoms
NH, (total) per
looo Cms. H2O.
Ag per
looo Gins. H2O.
Solid Phase.
0.0428
O.O25
AgCl
1.688
0.1308
"
3.782
0.372
"
3-945
0.378
"
5-io
0-574
"
5-33
0.609
"
5-545
0-633
"
6.26
0-754
" +2AgCl.3NH,
6.52
0-775
2AgC1.3NH,
8.28
0.848
"
11.78
0.980
"
12.68
1.030
"
12.96
I .090
K
14.47
1.039
«
Additional data for the above system at 25° are given by Bodlander and Fittig
(1901-02). These authors also give results showing the effect of KC1 and of
AgNOs on the solubility of AgCl in aqueous ammonia. Determinations at 15°
are given by Bodlander (1892),
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF:
Monomethyl Amine at 11.5°.
(Jarry.)
Gms. per 100 Gms. Solution.
Ammonia at o°.
(Jarry, 1899.)
Gms. per 100 Gms. Solution.
NH3 Gas.
i-45
2.94
5-6o
6.24
11.77
16.36
AgCl.
0.49
1.36
3-44
4
4.68
5-i8
NH3 Gas.
28.16
29.80
30.19
32.43
34.56
37-48
AgCl.
6.50
7.09
7-25
5-87
4-77
3-90
NH2CH3.
AgCl.
I.78
0.16
4.44
0.62
5-51
0.83
7.66
1.32
13.70
3-29
18.69
5-43
36.69
9-93
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIA.
(Longi, 1883; at 25°, Valenta, 1894; at 80°, Pohl, 1860.)
Solvent. t°.
Aq. Ammonia of o . 998 Sp. Gr. = 5%
0.96 Sp. Gr. = 10%
" o.986Sp. Gr.
= 3%
12
18
80
25
25
Gms. AgCl per
too Gms. Solvent.
0.233
7.84
1.49
1.40
7-58
607 SILVER CHLORIDE
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF METHYL
AMINE AND OF ETHYL AMINE AT 25°.
(Bodlander and Eberlein, 1903; Wuth, 1902; Euler, 1903.)
Results for Methyl Amine. Results for Ethyl Amine.
Mols. per Liter. Mols. per Liter.
Total Base.
I.OI7
0
AgCl.
.0387
Free Base.
0.940 (B. &E.)
Total Base.
0.483
0
AgCl.
.0314
Free Base.
0.420 (B. &
\
E.)
0-93
O
•0335
. . .
(E.)
0.200
0
.0115
0.177
"
0.508
0
.0178
0
.472
(B. & E.)
O. IOO
0
,0062
0.088
u
0.203
0
.0068
0
.189
lt
0.094
0,
,0048
. . .
(E.)
0.102
o
,0036
o
.0050
11
0.050
0
0029
0.044
(B. &
E.)
0.195
0.
00048
(W.)
0.103
0.
00824
(W.)
0.074
0,
00042
tt
0.0551
0.
000235
. . .
M
O.O2O
0.
00030
</f
O.OI27
0.
000114
11
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM
CHLORIDE.
(Schierholz, 1890; see also Vogel, 1874; Hahn, 1877.)
Solubility at 15°. Solubility at Different Temperatures.
Gms. per 100 Gms. Solution. Gms. per 100 Cms. Solution.
NH4C1.
AgCl.
I/ .
NH4C1.
AgCl.
IO
0.0050
15
26.31
0.276
14.29
0.0143
40
tt
0.329
17.70
0-0354
60
tt
0.421
19.23
0.0577
80
tt
0.592
21.91
O.IIO
90
tt
0.711
25-3I
0.228
IOO
U
0.856
28.45
0.340 (24.5)
no
tt
1-053
Sat. at ord. temp. p. 157 Sp. Gr. of 26.31% NH^Cl solution
at 15° = i. 08.
One liter aq. sol. containing 0.00053 gm. NH4C1 dissolves 0.001604 Sm-
at 25°.
One liter aq. sol. containing 0.00530 gm. NH4C1 dissolves 0.002379 gm. AgCl
at 25°. (Glowczynski, 1914.)
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM
CHLORIDE AT 25°. (Forbes, 1911.)
Gms. Equiv. per Liter. Gms. Equiv. per Liter. Gms. Equiv. per Liter.
'NH4C1. A^ 'NH4C1. A^ ' NH4C1. Ag^
0.513 0.000042 2.566 0.001425 4-777 0.0135
0.926 O.OOOII3 2.918 O.OO2IOO 4.902 0.01492
1.141 0.000172 3.162 0.002795 5-503 0.02404
1.574 0.000365 3-510 0.004029 5-764 0.03017
2.143 0.000842 4.363 0.009353
These determinations were made by gradually adding 0.25 n and o.oi n AgNOj
to the chloride solution and observing the point of initial opalescence
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF ALUMINIUM
AND AMMONIUM SALTS. (Valenta; see also Cohn, 1895.)
Gms. AgCl per 100 Gms. Solvent
Aq. Salt Solution. t°. of Concentration:
i : loo. 5 : loo. 10 : 100.
Aluminium Thiocyanate 25 ... ... 2.02
Ammonium Carbonate 25 ... ... 0.05
Thiocyanate 20 ... o . 08 o . 54
Thiosulfate 20 0.57 1.32 3.92
Calc. byCohn* 0.64 3.07 5.86
* See Note, p. 603.
SILVER CHLORIDE
608
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF BARIUM
CHLORIDE AND OF CALCIUM CHLORIDE.
(Forbes, 1911.)
Gms. Equiv.
per Liter.
Gms. Equiv.
per Liter.
Aq. Solution of:
Barium Chloride
t°. BaClj
Aq. Solution of: t°.
000186 Calcium Chloride 25
CaCl2 ^
2
3.264
O.
Ag.
001463
25
i.
2
248
O.
"
25
I,
, 610
0.
000339
25
3
•737
O.OO2I82
H
25
2
.676
0.
001274
2S
4
•033
O.
002802
tt
25
3
. 260
0.
002366
2S
4
0.
004175
CaCU
2
25
5
.005
0.
005823
Calcium Chloride
25
i
.748
0.
000289
I
3
•512
o . 000964
u
25
2
.2OI
0.
000501
25
3
.320
0.
001514
u
25
2
.741
0.
000900
35
3
. 221
0.
001806
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
CHLORIC ACID AT 25°.
(Forbes, 1911.)
Gms. Equiv. per Liter,
licl Ag!
0.649 O.OO0032
1.300 O.OOOI26
I.QII O.000266
Gms. Equiv. per Liter.
Gms. Equiv. per Liter.
HC1.
2.149
2-975
Ag.
0.000374
0.000814
0.001358
HC1.
4.182
4-735
5.508
Ag.
0.002147
0.003168
0.005126
O.OIW
The determinations of Forbes were made by gradually adding 0.25 n and o.c
AgNOs to the chloride solution and observing the point of initial opalescence.
Oneliterof I per cent aq.HCl dissolve 0.0002 gm.AgCl at 21°. (Whitby, '10.)
1 5 0.0033 "
" 10 . " (0.0555)0.0740 "
NOTE. — The determinations of Whitby were made by a colorimetric method
which was based upon the observation that the color produced by heating a solution
of a silver salt with sodium hydroxide and certain organic compounds such as dex-
trin, glycerol, starch, sugar, etc., is proportional to the amount of silver present.
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS HYDROCHLORIC ACID SOLU-
TIONS AT ORDINARY TEMPERATURE.
(Pierre, 1847; Vogel.)
Solvent.
Cone. HC1 + Aq.
i vol. Cone. HC1 + i vol. H2O
Sat. HC1 Sp. Gr. 1.165
Gms. AgCl
per Liter.
1.6
2.98
(at b. pt.) 5 . 60
Solvent.
Gms. AgCl
per Liter.
ioo vol. sat. HC1 + 10 vol. H2O o. 56
+ 20 " 0.18
+ 30 " 0.09
+ 50 " 0.035
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF MERCURIC
NITRATE AT 25°,
(Morse, 1902.)
A101S.
HgN03(HNO3)
per Liter.
Mols. AgCl
per Liter.
Gms. AgCl
per Liter.
MOIS.
HgNOaCHNOa)
per Liter.
Mols. AgCl
per Liter,
Gms. AgCl
per Liter.
O.OIOO
0 . 0043 2
0.620
0.050
0.00914
I.3IO
0.0125
0.00499
0-7I5
O. IOO
0.01395
2
0.025
o . 00690
0.990
I
0.04810
6.896
Since HNO3 was present in all cases, its influence on the solubility was examined.
It was found that no appreciable differences were obtained with concentrations
varying between o.i and 2 normal HNO3. Both crystallized and amorphous
silver chloride gave identical results.
669
SILVER CHLORIDE
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SALT SOLUTIONS.
(Vogel; Hahn; Valenta )
Salt Solution.
Barium Chloride
Barium Chloride
Barium Sulphocyanide
Calcium Sulphocyanide
Calcium Chloride
Calcium Chloride
Copper Chloride
Ferrous Chloride
Ferric Chloride
Manganese Chloride
Magnesium Chloride
Magnesium Chloride
Magnesium Chloride
Strontium Chloride
Zinc Chloride
Potassium Chloride
Potassium Chloride
Potassium Cyanide
Potassium Cyanide
Potassium Sulphocyanide
Sodium Chloride
Sodium Chloride
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF NITRIC
ACID AT 25°.
(Glowczynski, 1914-)
Mols. per Liter. Cms. per Liter.
Cone, of Salt.
t o Gms. AgCl per
loo Gms. Solution.
27.32%
24-5
0.057
(H.)
saturated
ord. temp.
0.014
(Vg.)
io : 100
25
0-20
(VI.)
io : 100
25
0.15
(VI.)
41.26%
24-5
0-571
(H.)
saturated
ord. temp.
0-093
(Vg.)
"
24-5
0-053
(H.)
n
it
0.169
(H.)
"
"
O-OO6
(H.)
<(
it
0.013
(H.)
50 : 100
25
0.50
(VI.)
36.35%
24 5
0-531
(H.)
saturated
ord. temp.
O.I7I
(Vg.)
"
it
0.088
(Vg.)
"
24-5
0.0134
(H.)
it
ord. temp.
0-0475
(Vg.)
24-95%
19.6
0.0776
(H.)
5 *• 100
25
2-75
(VI.)
5:100
25
5-24
(Cohn*)
io: 100
25
O.II
(VI.)
saturated
ord. temp.
0.095
(Vg.)
25-95%
19-6
0-105
(H.)
* See Note, p.
603.
HNO3.
AgCl.
0.0005
I.I5.IO-5
O.OOI
i.ig.io"5
0.01
i . 24 . io~5
0.30
I.57.IO-5
' HN03.
AgCl.
0.0315
0.001647
0.063
O.OOI7O5
0.630
0.00176
18.9
0.00225
94-5
0.00245
1.71.10-°
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
CHLORIDE AT 25°.
(Forbes, 1911.)
Gms. Equiv. per Liter. Gms. Equiv. per Liter.
(Glowczynski, 1914.)
Mols. per Liter. Gms. per Liter.
KC1.
I. Ill
Ag.
0.000141
KC1. Ag.
2.850 0.001845
KC1.
AgCl.
KC1.
AgCl.
1.425 0.000235 3.081 0.002435
0.000391 3.424 0.003602
2.022 0.00o6l6 3.843 0.005725
3.I6.IO"5 I.28.IO""6 0.00236 0.001836
6.32.IQ-6 I.52.IQ-6
2.O. IO ~* 2. 13. IO"5
4.0. io ~* 2.24. lo"5
0.00471 0.002178
O.OI49I 0.003052
0.02984 0.003209
2.396 0.001050 3.325 o.ooi734(at i°)
2.628 0.001390 2.955 0.002 786 (at 35°)
The determinations of Glowczynski were made by the method described in
Note, on p. 605. The determinations of Forbes were made by gradually adding
0.25 n and o.oi n AgNO3 to the chloride solution and observing the point of
initial opalescence.
One liter 4 n aq. KC1 dissolves 0.00637 Sm- mol. = 0.915 gm. AgCl at 25°.
(Hellwig, 1900.)
SILVER CHLORIDE 610
SOLUBILITY OP SILVER CHLORIDE IN AQUEOUS SOLUTIONS OP
POTASSIUM CHLORIDE AT 15°.
(Schierholz — Sitzber. K. Akad. Wiss. (Vienna) 101, ab, 8, '90.)
Grams per too Grams Grams per 100 Grams
Solution. Solution.
KC1. AgCl. KC1. AgCl.
lo.o o.ooo 22.47 0-045
14.29 O-OO4 24.0 O.O72
16.66 0.008 25.0 0.084
20.00 0.020 Sp. Gr. of 25% KC1 sol,= 1.179
MIXTURES OF SILVER CHLORIDE AND SILVER HYDROXIDE IN EQUI-
LIBRIUM WITH AQ. POTASSIUM HYDROXIDE SOLUTIONS AT 25°.
(Noyes and Kohr — J. Am. Ch. Soc. 24, 1144, '02.)
Normality Millimols per Liter. Grams per Liter.
ofKOH. KC1. KOH.' KC1. KOH. AgCl.
0-333 3-4I4 347-8 0.255 IO-°5 0.4896
0-065 0-598 65.0 0-0446 2.OO 0-0828
SOLUBILITY OF SILVER CHLORIDE IN AQ. SODIUM CHLORIDE SOLUTIONS.
(Schierholz; Vogel; Hahn.)
Solubility at 15°. Solubility at Different Temperatures
Gms. per 100 Gms, + 0 Gms. AgCl per 100 Gms.
Solution. Solution in:
NaCl. AgCl. 14% NaCl 26.3% NaCl.
io.o 0.0025 15 0.007 0.128
14.29 0.0071 30 O.OIT 0.132
18.18 0.0182 40 0-014 0.158
21.98 0.0439 50 0.023 0.184
23-53 0.0706 70 0.042 0.263
25.64 0.103 80 0.054 0.315
26.31 0.127 90 0.069 0.368
100 0.090 o 460
Sp.Gr. of 26.31% NaCl sol. = 1.207. 109 0.107(104°) 0.571
SOLUBILITY AT 20°, 50°, AND 90° (CALC. FROM ORIGINAL).
(Barlow — J. Am. Chem. Soc 28, 1446, '06.)
Gms. NaCl Gms. AgCl dissolved per 100 cc. Gms. NaCl
per loo cc. Solution at: per I00 cc.
Gms. AgCl dissolved per 100 cc.
Solution at:
Solution.
20°.
50°.
90°
Solution.
'20°.
50°.
00°.
3-43
0
.OOOlS
0.0016
0
.0067
"•5
0
.0031
0
.0124
0.0436
4.60
0
OO025
0.0025
0
• OIOO
i5-3
0
.009O
0
.0191
0.0732
5-75
0
.00047
0.0034
0
•0135
23.0
0
•0313
0
.0889
0.1706
7.67
0
OOI25
0.0058
0
.0236
Results are also given for the solubility of silver chloride in aqueous sodium
chloride solutions containing hydrochloric acid.
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SODIUM CHLORIDE AT 25°.
(Forbes, 1911.)
Gms. Equiv. per Liter. Gms. Equiv. per Liter. Gms. Equiv. per Liter.
[NaCl]. [Ag]Xio». ' [NaCl]. [AglXioS.' ' [NaCl]. [Ag]Xio3.'
0.933 0.086 2.272 0.570 3-747 2.462
1.190 0.130 2.658 0.851 3-977 2.879
1.433 0.184 2.841 1.040 4-363 3-810
1.617 0-245 3-270 1-583 4-535 4-298
1.871 0.348 3.471 1.897 5.039 6.039
6n SILVER CHLORIDE
SOLUBILITY OF SILVER CHLORIDE IN AQ. SODIUM NITRATE SOLUTIONS.
Cms, per 100 Cms. HtO. Cms. per 100 Cms. H2O.
NaN03. AgCl. ' NaN03. AgCl. '
5 0.787 0.00086 15-20 0.393 0.00096
18 0.787 0.00146 0.787 0.00133
30 0.787 0.00233 2.787 0.00253
45-55 0-787 0.00399 (Mulder.)
One liter aq. 3 n AgNO3 dissolves 0.0056 gm. mols. = 0.8 gm. AgCl at 25°.
(Hellwig, 1900.)
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SODIUM SULFITE SOLUTIONS
AT 25°.
(Luther and Leubner, 1912.)
Gms. Formula Weight per Liter. Gms. Formula Weight per Liter.
S03". Ap! S03". Ap!
0.080 o.on 0.483 0.059
0.106 0.017 0.470 0.070
0.220 0.033 0.652 0.103
0.234 0.036 0.890 O.I4O
0.478 0.057 0.937 0.142
The AgCl was prepared by precipitating dilute AgNO3 with alkali chloride at
the b. pt. The resulting solid corresponded to the granular modification of Stas.
About one hour constant agitation was allowed for attainment of equilibrium.
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
THIOSULFATE, ETC.
(Valenta; Cohn; Richards and Faber, 1899.)
Gms. AgCl per 100 Gms. Aq. Solutions of Concentration:
Salt Solution. t°. , » N
i : zoo. 5 : 100. 10 : 100. 15 : 100. 20 : 100.
Sodium Sulfite 25 ... ... 0.44 ... 0.95
Sodium Thiosulfate 20 0.40 2 4.10 5.50 6.10
" Calc. by Cohn.* 0.38 1.83 3.50 5.02 6.41
Sodium Thiosulfate 35 9.o8f
Thiocarbamide 25 ... ... 0.83
Thiocyanimine 25 0.40 1.90 3.90
* See Note, p. 603. t Gms. per 100 cc. solution (R. and F.).
SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS STRONTIUM CHLORIDE AT 25°.
(Forbes, 1911.)
Gms. Equiv. per Liter.
Gms. Equiv. per Liter.
Gms. Equiv. per Liter.
SrCl2
2
AgXio».
' SrCl2-
2
AgXioS.
SrCl2-
2
AgXio*.
0.550
0-033
1.818
0.348
3-494
2.018
0.989
0.092
2.140
0.510
4-I52
3-594
1-359
0.173
2.476
0-747
5.216
8.174
1-572
0.236
2.992
1.252
5-775
12.040
The determinations were made by gradually adding 0.25 n and o.oi n AgNOs to
the chloride solution and observing the point of initial opalescence.
One liter of 4.777 n ZnCl2 solution dissolves 0.000364 mol. AgCl at 25°.
(Forbes, 1911.)
Fusion-point data are given for the following mixtures.
AgCl + Agl. (Monkemeyer, 1906.)
AgCl + Ag2S. (Truthe, 1912; Sandonnini, 1912.)
AgCl + NaCl. (Sackur, 1913; Botta, 1911; Sandonnini, 1911, 1914.)
AgCl + T1C1. (Sandonnini, 1911, 1914.)
SILVER CHLORIDE 612
SOLUBILITY OF SILVER CHLORIDE IN PYRIDINE.
(Kahlenberg and Wittich, 1909.)
Cms. AgCl Cms. AgCl c .. .
t°. per 100 Cms. Solid Phase. t°. per 100 Gms. p.?
Pyridine. Pyridine. Phase"
— 57 EutCC. ... AgC1.2C6H6N+C6H6N O 5.35 AgCl
— 49 0.77 AgCl.2C6H6N 10 3.17
— 35 0.99 20 I.QI
-30 1.36 " 30 1.20
— 25 1. 80 40 0.80
— 22 2.20 ". 50 0-53
— tr.pt. 2.75 " +Agd.c6H5N 60 0.403
— 20 3.75 AgCLCsHsN 70 0.32
-18 3.85 " 80 0.25
-10 4.35 " 90 0.22
— 5 5.05 ioo 0.18
— I 5.60 " 110 0.12
SILVER CHROMATE Ag2CrO4.
One liter of water dissolves 0.026 gm. Ag2CrO4 at 18°, and 0.020 gm. at 25°.
(Abegg and Cox, 1903; Kohlrausch, 1904-05.)
One liter H2O dissolves 0.029 gm. AgiCrO4 at 25°. (Schafer, 1905.)
One liter of H2O dissolves 0.0142 gm. Ag2CrO4 at 0.26°; 0.0225 gm. at 14.8°,
0.036 gm. at 30.7° and 0.084 gms- at 75°- (Kohlrausch, 1908.)
One liter H2O dissolves 0.0256 gm. at 18°, 0.0341 gm. at 27° and 0.0534 Sm- at
50°, determined by a colorimetric method (see Note, p. 608). (Whitby, 1910.)
SOLUBILITY OF SILVER CHROMATE IN AQUEOUS AMMONIA AT 25°.
(Sherrill and Eaton, 1907.)
Mols. NHiOH per Liter o.oi 0.02 0.04 0.08
Mols. X io3 Ag2CrO4 per Liter 2.004 4.169 8.595 17.58
SOLUBILITY OF SILVER CHROMATE IN AQUEOUS NITRIC ACID AT 25°.
(Sherrill and Russ, 1907.)
Mols. HNO3 Milliatoms per Liter. Solid
per Liter. Cr. Ag. Phase.
Mols. HNO3 Milliatoms^ per Liter.
per Liter. Cr. Ag.
O
.OI
3
•157
6.315 Ag2CrO4
O.O6
6
•833
.
O
.015
3
•730
"
O,
.07
7
•333
.
0.02
4
.177
8.356
O.
•075
7
•477
14
•85
0
.025
4
.567
. . .
0,
,08
7
.260
i5
•45
0
•03
5
.200
... "
0,
,1(7
5
•647
19
.01
/ O
.04
5
•803
11.62
O.
13
4
•293
23
.89
0
•93
6
.380
... "
O,
,14
3
.948
25
•63
Solid
Phase.
Ag,CrO4
One liter 65% aqueous alcohol dissolves 0.78 X io~4 gms. equivalents = 0.0129
gm. Ag2CrO4 at room temp. (?). (Guerini, 1912.)
SOLUBILITY OF SILVER CHROMATE IN AQUEOUS SOLUTIONS OF NITRATES AT 100°.
(Carpenter, 1886.)
Gms. Salt Gms. Ag2CrO4
Solvent. per too cc. per ioo cc.
H2O. Solution.
Water o o . 064
Sodium Nitrate 50 o . 064
Potassium Nitrate 50 0.192
Ammonium Nitrate 50 0.320
Magnesium Nitrate 50 0.256
6i3 SILVER CHROMATE
SILVER (Di) CHROMATE Ag2Cr2O7.
One liter of aqueous solution contains 0.00019 gni. mol. or 0.083 gm- Ag2Cr2O7
at 15°. (Mayer, 1903.)
SOLUBILITY OF SILVER DICHROMATE IN AQUEOUS NITRIC ACID AT 25°.
(Sherrill and Russ, 1907.)
Milliatoms per Liter.
Solid Phase.
>er Liter.
Cr.
Ag.
0
0.01
O.O2
32.20
25.06
2O. 21
5-390
6.131
7.148
0.04
0.06
13-59
II. 10
9-529
II. I
0.08
II .1
II. I
0.08+0.1 AgNO3
6.625
. . ...
At the lower concentrations some of the dichromate is converted into solid
chromate.
SILVER CITRATE C6H5O7Ag3.
loo gms. H2O dissolve 0.0277 gm. CeHsO/Ags at 18°, and 0.0284 Sm- at 25°-
(Partheil and Hubner, 1903.)
SILVER CYANIDE AgCN.
One liter of aqueous solution contains 0.000043 gm. AgCN at 17.5° and 0.00022
gm. at 20° (by Conductivity Method). (Abegg and Cox; Bottger, 1903.)
SOLUBILITY OF SILVER CYANIDE IN AQUEOUS AMMONIA SOLUTIONS.
(Longi, 1883.)
100 gms. aq. ammonia of 0.998 Sp. Gr. = 5%, dissolve 0.232 gm. AgCN at 12°.
100 gms. aq. ammortia of 0.96 Sp. Gr. = 10%^ dissolve 0.542 gm. AgCN at 18°.
One liter aq. 3 n AgNO3 dissolves 0.0091 gm. mol. = 1.216 gm. AgCN at 25°.
(Hellwig, 1900.)
Fusion-point data for mixtures of AgCN + NaCN are given by Truthe (1912).
SILVER FERRICYANIDE Ag3FeCN6.
3FeCN6 at 20°. See Note, p
fhitby, 1910.)
One liter H2O dissolves 0.00066 gm. Ag3FeCN6 at 20°. bee JNote, p.
(Wl
SILVER SODIUM CYANIDE AgCN.NaCN.
100 gms. H2O dissolve 20 gms. at 20°, and more at a higher temperature. 100
gms. 85% alcohol dissolve 4.1 gms. at 20°. (Baup, 1858.)
SILVER THALLOUS CYANIDE AgCN.TICN.
100 gms. H2O dissolve 4.7 gms. at o°, and 7.4 gms. at 16°. (Fronmuller, 1878.)
SILVER FLUORIDE AgF.2H2O.
SOLUBILITY IN WATER.
(Guntz and Guntz, Jr., 1914.)
— 14.2 EutCC. 60 Ice+AgF.4H2O 25 1 79 -5 AgF.2H2O
+ 18.5 165 AgF.4H20 28.5 215
18.65 z^9-5 " +AgF.2H2O 32 193
2O 172 AgF.2H2O 39-5 222 " +AgF
24 178 " I08 205 AgF
Two unstable hydrates, AgF.H2O and 3AgF-5H2O were also obtained.
100 gms. H2O dissolve 181.8 gms. AgF at 15.8°, di$.& of Sat. Sol. = 2.61. (Gore, 1870.)
SILVER FLUORIDE
614
SOLUBILITY OF SILVER FLUORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
FLUORIC ACID AT O° AND AT 24°.
(Guntz and Guntz, Jr., 1914-)
Results at 24°.
Results
Gms. per ioo Gms. H2O.'
Solid Phase.
AgF.
HF.
87-5
0.40
AgF.4H2O
89.4
2.0O
"
93-8
3-97
ii
Il8.5
9.60
"
156
14
" +AgF.
159
17.2
AgF.aH.O
185
24
"
I89
25-7
AgF
188
29-5
"
196
39-8
"
142.1
52
AgF.2H2O
121.75
57-2
M
94-93
66.57
"
173-75
0.4
3AgF.sH2O
174
3-6
"
AgF.
HF.
•» ouiiu iruasc.
I78
O
AgF.2H2O
178.5
i-73
"
I77-65
5-42
*!
179-5
IO
"
189.5
13-4
ii
I9I-5
14-3
" +AgF(?)
207
0-15
3 AgF.5H20
2O6.2
1-25
"
202.5
7-9
ii
198.6
12.65
"
195-5
11.7
AgF.H,O
194-5
13
"
189.5
18.8
3AgF.SH20+AgF(?)
193
36.6
AgF
193-5
16
Additional determinations at other temperatures are given.
SILVER FULMINATE CAg^NO^CN.
One liter of aqueous solution contains 0.075 gm. C2Ag2N2O2 at 13°, and 0.180
gm. at 3Or (Holleman, 1896.)
SILVER HEPTOATE (Onanthylate) AgC7H13O2.
SOLUBILITY IN WATER.
(Landau, 1893; Altschul, 1896.)
^o Gms. AgCyHisOj per ioo Gms. H2O. ^.o
O O . 0635 (Landau) O . 0436 (Altschul) 50
10 0.0817 0.0494 60
20 0.1007 °-°555 7°
30 o.i 206 0.0617 80
40 0.1420 0.0714
Gms.
ioo Gms.
0.1652 (Landau) O . 08 5 8 (Altschul)
0.1906 0.1036
0.2185 °-I35I
0.2495 0.1688
SILVER IODATE AgIO3.
One liter of aqueous solution contains 0.04 gm. or 0.00014 &m- mol. at i8°-2O°,
and 0.05334 gm. or 0.000189 gm- mol. at 25°.
(Longi; Bottger; Kohlrausch; Noyes and Kohr, 1902.)
The solubility of. silver iodate in water, determined by a colorimetric method
(see Note, p. 608), was found by Whitby (1910) to be 0.039 gm- AgIO3 per
liter at 20°. Determinations reported by Sammet (1905) made by a chain cell
method, gave 0.0611 gm. AgIO3 per liter at 25° and 0.1849 Sm- at 6o°-
One liter of H2O dissolves 0.0275 gm- AgIO3 at 9.43°, 0.039 gm. at 18.4° and
°-°539 gm- at 26.6°. (Kohlrausch, 1908.)
SOLUBILITY OF SILVER IODATE IN AQUEOUS SOLUTIONS OF AMMONIA AND
OF NITRIC ACID AT 25°.
(Longi, 1883.)
ioo gms. aq. ammonia of 0.998 Sp. Gr. = 5% dissolve 2.36 gms. AgIO3.
ioo gms. aq. ammonia of 0.96 Sp. Gr. = 10% dissolve 45.41 gms. AgIO3.
ioo gms. aq. nitric acid of 1.21 Sp. Gr. =35% dissolve 0.096 gm. AgIO3.
6i5
SILVER IODATE
SOLUBILITY OF SILVER IODATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT 25°,
(Hill and Simmons, 1909.)
Normality of
Aq. HNO,.
O
0.125
0.250
0.500
Cms. AglOj
per Liter.
0.0503
o . 0864
0.1075
O.I4I4
Normality of
Aq. HNO3.
I
2
4
8
Cms. AglOj
per Liter.
0.2067
0.3319
0.6085
1.587
The solubility of the amorphous modification of AglOs is considerably higher
than that of the crystalline, but the amorphous product rapidly becomes crystalline
and correct results are soon obtained.
SILVER IODIDE Agl.
One liter of aqueous solution contains 0.0000028 gm. Agl at 2O0-2§°.
(Average of several determinations by Kohlrausch, Abegg and Cox, etc., Holleman gives higher figures.)
One liter of water dissolves 0.0000253 Sm- Agl at 60°, determined by a chain
cell method (Sammet, 1905). This author also gives data for the solubility of
Agl in i n and o.i n KI solutions at 60°.
Per cent Con-
centration of Aq.
Ammonia.
7
10
SOLUBILITY OF SILVER IODIDE IN AQUEOUS AMMONIA.
Authority.
d of Aq.
Ammonia.
Gms. Agl
per Liter.
0.971 1 6 0.045 (Ladenburg, 1902.)
0.960 12 0.035 (Longi, 1883.)
2O 0.926 l6 O.l66 (Baubigny, 1908.)
Baubigny used a sealed tube and noted the first appearance of crystallization
of Agl in mixtures of known compositions.
SOLUBILITY OF SILVER IODIDE IN AQUEOUS MERCURIC NITRATE AT 25°.
(Morse, 1902.)
Mols. Hg(NOs),
per Liter.
Mols. Agl
per Liter.
Gms. Agl Mols. Hg(NO3),
per Liter. per Liter.
Mols. Agl per
Liter, j
Gms. Agl
per Liter.
O.OIO
o . 00340
0.800
0.050
O.0074O
1-737
0.0125
0.00358
0.841
0. IOO
o. 01161
2.730
0.025
0.00476
i.zxS
I
O.I070O
25. 160
Since HNOs was present in all cases its influence on the solubility was examined.
It was found that no appreciable differences were obtained with concentrations
varying between o.i and 2 n HNO3. Both crystallized and amorphous silver
iodide gave identical results.
SOLUBILITY OF SILVER IODIDE IN AQUEOUS SOLUTIONS OF POTASSIUM
IODIDE AND OF SILVER NITRATE AT 25°.
(Hellwig, 1900.)
In Aq. KI Solutions.
In Aq. AgNO3 Solutions.
fols. KI
Mols. Agl
Gms. Agl
Mols.
AgN03
Mols. Agl
Gms. Agl
Solid
er Liter.
per Liter.
per Liter.
per
Liter.
per Liter.
per Liter.
Phase.
0.
335
0.000363
o
0853
O.
20
O
OO0289
O
.068
Agl
0.
586
O.O02I8
0
5"
0.
35
0
000532
0
.121
0.
734
0.0044
I
032
0.
50
O
OOI27
O
.299
"
008
O.OI4I
3
32
0.
70
O
00362
0
.850
"
018
0.0148
O
47
I.
215
0
0131
3
.08
AgjINO,
406
0.0535
12
55
I.
63
0
0267
6
.26
"
486
0.0658
15
46
2.
04
O
0458
IO
•9
«
6304
0.102
24
01
2.
54
0
0678
16
. i
AftKNO,),
.
937
0.198
46
42
3-
75
0
141
33
.2
4-
69
0
227
53
.2
«
5-
90
O
362
85
u
SILVER IODIDE
616
SOLUBILITY OF SILVER IODIDE IN AQUEOUS SALT SOLUTIONS.
(Valenta, 1894; Cohn, 1895.)
Aq. Salt. Solution. t°.
Sodium Thiosulfate 20
" Calc. by Cohn.*
Potassium Cyanide 25
" Calc. by Cohn.*
Sodium Sulfite 25
Ammonium Thiocyanate 20
Calcium
Barium
Aluminium "
Thiocarbamide
Thiocyanime
Gms. Agl per 100 Cms. Aq. Sol. of Concentration:
i : ioo.
5 : ioo.
10 : ioo.
15 : ioo.
20 : ioo.
0.03
0-15
0.30
0.40
0.60
0.623
2.996
5.726
8.218
10.493
8.28
. . .
8.568
. . .
. . .
. . .
. . .
O.OI
. . .
0.02
O.O2
0.08
0.13
...
0.03
O.O2
. . .
. . .
. . .
O.O2
...
...
0.79
. . .
. . .
0.008
0.05
O.O9
25
25
25
25
25
* See Note, p. 603.
SOLUBILITY OF SILVER IODIDE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE,
POTASSIUM BROMIDE AND OF POTASSIUM IODIDE AT 15°.
(Schierholz, 1890.)
In Sodium Chloride.
Gms. per 100 Gms. Solution.
In Potassium Iodide.
Gms. per 100 Gms. Solution.
NaCl.
26.31
25.00
Agl.
O.O244
O.OOO72
KI.
59.16
Agl.
53-^3
57-15
40-0
50.0
25.0
4O.O
13.0
33-3
7-33
25.0
21.74
20-0
2-75
1.576
0.80
In Potassium Bromide.
Gms. per IPO Gms. Solution.
KBr Agl
30.77 0.132
ioo gms. sat. silver nitrate solution dissolve 2.3 gms. Agl at 11°, and 12.3 gms.
at b. pt.
ioo gms. pyridine dissolve o.io gm. Agl at 10°, and 8.60 gms. at 121°.
» (von Laszcynski, 1894.)
SOLUBILITY OF SILVER IODIDE IN AQUEOUS SODIUM IODIDE AT 25°.
(Krym, 1909.)
Gms. per ioo Gms. H2O.
Nal.
59-29
67.47
Agl.
31.21
28.52
I34-I
156.9
99-54
124.6
179.8
196.3
150
134.8
223.7
122
Solid Phase.
Gms. per ioo Gms. H2O.
Agl
" +AgI.NaI.3*H2O
AgI.NaI.3*H2O
Nal. Agl.
ouuu jriiasc.
226 120-9
AgI.NaI.3§HjO+NaI
222-7 H2. 1
Nal
214.7 90.84
"
203.9 59.48
"
194.5 31.10
"
185.52 o
"
The above table was calculated from the original results which are expressed in
mols. per 1000 mols. H2O.
Fusion-point data for mixtures of Agl + HgI2 are given by Steger (1903).
Results for Agl + Nal are given by Sandonnini and Scarpa (1913).
Laurate.
Myristate.
Palmitate.
Stearate.
35
0.007
O.OO4
O.O04
50
. . .
O.OO7
O.OO6
O.OO4
25
0.009
0.008
O.007
O.OO7
So
0.009
0.008
O.OO7
O.007
15
0.074
0.063
0.060
0.051
25
0.072
0.067
0.059
0.052
35
0.078
0.071
O.062
0.055
50
0.083
0.073
0.066
0.000
15
O.OIO
0.009
O.OO9
0.007
617 SILVER LAURATE
SILVER LAURATE, MYRISTATE, PALMITATE and STEARATE
SOLUBILITY OF EACH, DETERMINED SEPARATELY, IN WATER AND OTHER
SOLVENTS AT SEVERAL TEMPERATURES.
(Jacobson and Holmes, 1916.)
Cms. each Salt per too Gms. Solvent.
Solvent.
Water
u
Abs. Ethyl Alcohol 25
a ii
Methyl Alcohol
Ether
SILVER LEVULINATE (Acetyl propionate) CH3.COCH2CH2COOAg.
SOLUBILITY IN WATER.
(Furcht and Lieben, 1909.)
jo Gms. per loo Gms. Sat. Solution.
8 o. 5363 (white salt) o. 5195 (yellow salt)
9 0.5166 0.5372
14-15 0.6078 0.6448
99-6 3-49 3-70
SILVER MALATE C4H4O5Ag2.
100 gms. H2O dissolve 0.0119 Sms. at 18°, and 0.1216 gm. at 25°.
(Partheil and Hiibner, 1903.)
SILVER NITRATE AgNO3.
SOLUBILITY IN WATER.
(Etard, 1894; Kremers, 1854; Tilden and Shenstone, 1884.)
Gms. AgNO3 per 100 Gms. Gms. AgNO3 per 100 Gms.
Solution.
Water.
Solution.
Water.
~ 5
48 (Etard)
50
79 (Etard)
82
455
0
53
55
122
60
8x.
5
84
525
IO
62
63
170
80
85.
5
87
669
20
68
69
222
IOO
88.
5
90*
952
25
70.
5
72
257
120
9i
95
1900
30
72.
5
75
300
140
93-
5
. . .
. . .
40
76.
5
79
376
160
95
ioo gms. sat. aq. solution contain 47.1 gms. AgNO3 at —7.3° (= Eutectic).
(Middleberg, 1903.)
IOO gms. sat. aq. sol. contain 65.5 gms. AgNOs at 15.5°. (Greenish and Smith, 1903.)
IOO gms. sat. aq. sol. contain 73 gms. AgNOs at 30°. (Schreinemakers and de Baat, igioa.)
SOLUBILITY OF SILVER NITRATE IN AQUEOUS NITRIC ACID AT 25°.
(Masson, 1911.)
4. of Sat.
Gm. Mols
. per Liter.
Gms. AgNO3
4; of Sat.
Gm. Mols.
per Liter. Gms. AgNO,
Sol.
' HN03.
AgNOj.
per Liter.
Sol.
' HNOS.
AgN03.
per Liter.
2.3921
0
10.31
1752
I . 4980
4-497
2.590
440.1
2.2754
0.4042
9-36
1591
I.4I95
5-992
1.698
288.6
2.1243
0.962
8.08
1373
1.3818
8.84
0.843
143-2
1.9402
1.698
6-54
IIII
1.3976
12.53
0-347
58.96
T.7052
2.834
4.526
769.1
ioo gms. 2HNOS.3H2O dissolve 3.33 gms. AgNO3 at 20°, and 16.6 gms. at 100°.
ioo gms. cone. HNOi dissolve 0.2 gm. AgNOj. (Schultz, 1860.)
SILVER NITRATE 618
SOLUBILITY OF MIXED CRYSTALS OF SILVER NITRATE AND SODIUM NITRATE
IN AQUEOUS ETHYL ALCOHOL.
(Hissink, igoo.)
Results at 25° in Results at 50° in
Aq. C2H6OH of fa = 0.945 (37 wt. %). Aq. C2H6OH of d17 = 0.859 (75 wt. %).
Gms. per 100
Gms. Sol.
Wt. per cent in
Mix Crystals.
Gms. per 100
Gms. Sol.
Wt. per cent in
Mix Crystals.
' AgNO3.
NaN03.
AgN03.
NaNO3
AgN03.
NaN03.
AgNO3.
NaNOs
47-32
o
• O
100
O
.0
29
.78
o.o
100
o.o
44-01
8
,78
99-1
O
•9
27
•9
2-5
99
5
°-5
36.78
20
.42
42.9
57
.1
26
•4
4.2
99
•3
0.7
29.97
23
.2
33-6
66
•4
23
.0
6.3
42
9
57-i
24.56
24
.82
27.6
72
•4
18
•3
7.1
3*
.0
69.0
8.02
26
.41
9-9
90
.1
9
•5
8.3
17
•5
82.5
o.o
26
•77
o.o
100
.0
0
.0
8.54
o
.0
100. 0
Very extensive data for equilibrium in the system silver nitrate, succinic acid
nitrile and water are given by Middelberg (1903). This author first gives data
for the ternary systems and then results for isotherms of the ternary system at
o°, 12°, 20°, 25° and 26.5°. A number of determinations for higher temperatures
are also given. The following compounds of succinic nitrile and silver nitrate
were identified; C2H4(CN)2.4AgNO3, C2H4(CN)2.2AgNO3, C2H4(CN)2.AgNO3,
2C2H4(CN)2.AgN03.H20, and 4[2C2H4(CN)2.AgNO3]H2O. Additional data for
this system are also given by Timmermans (1907).
SOLUBILITY OF SILVER NITRATE IN ALCOHOLS.
(de Bruyn, 1892.)
100 gms. abs. methyl alcohol dissolve 3.72 gms. AgNO3 at 19°.
100 gms. abs. ethyl alcohol dissolve 3.10 gms. AgNO3 at 19°.
SOLUBILITY OF SILVER NITRATE IN AQUEOUS ETHYL ALCOHOL,
(Eder, 1878.)
Sp. Gr.of Aq. Volume Gms. AgNO3 per 100 Gms. Aq. Alcohol at:
Alcoholic per cent / * s
Mixture- Alcohol. 15°. 50°. 75°.
0.815 95 3.8 7.3 18.3
0.863 80 10.3 ... 42.0
0.889 70 22.1
0.912 60 30.5 58.1 89.0
0.933 50 35.8
0.951 40 56.4 98-3 160.0
0.964 30 73.7
0-975 2° 107.0 214.0 340-0
0.986 10 158-0
ioo gms. of a mixture of I vol. (95%) alcohol + I vol. ether dissolve 1.6 gms.
AgNO3 at 15°.
ioo gms. of a mixture of 2 vols. (95%) alcohol + I vol. ether dissolve 2.3 gms.
AgNO3 at 15°.
ioo gms. H2O sat. with ether dissolve 88.4 gms. AgNO3 at 15°. (Eder, 1878.)
ioo gms. acetone dissolve 0.35 gm. AgNO3 at 14°, and 0.44 gm. at 18°.
(von Lasczynski, 1894; Naumann, 1904.^
6 19 SILVER NITRATE
SOLUBILITY OF SILVER NITRATE IN SEVERAL SOLVENTS.
Solvent.
Acetonitrile (anhydrous)
a
1 8 290
ord. temp, about 150
Authority.
(Naumann and Schier, 1914.)
(Scholl and Steinkopf, 1906.)
Benzonitrile
18 about 105
(Naumann,
1914.)
Benzene
35
O.022
(Linebarger
, 1895.)
{(
40.5
0.044
Hydrazine
(anhydrous)
ord. temp.
I (with decomp.) (Welsh and Broderson, 1915.)
SOLUBILITY OF SILVER NITRATE IN
PYRIDINE.
(Kahlenberg and Brewer, 1908.)
t°.
Gms. AgNOj
per 100 Gms.
Solid Phase.
t°.
Gms. AgNO,
per too Gms.
Solid Phase.
CjHjN.
C^N.
-48.501.
pt. o
C5H6N
45
62 . 26 AgNOj.sQHjN
-50-5
3
"
46
63 . 09
-53
6
"
47
66.35 '
|
-59
9
«
48
70.85 '
—65 Eutec.
"+AgNO3.6C5H8N
48.5tr.
pt. ...
[+AgNO,.2CsHbN
-51-25
II. I
AgNO,.6CsHsN
45
69.85
AgNOa.jQHiN
-44
ix. 7
"
50
72.25
"
-40
12.2
"
60
78.60
«
-35
12.6
"
70
89.10
"
-30
13-9
<(
80
121. 21
«
-25
I7.6
"
87
215.02
"
— 24 tr. pt
. ...
"+AgN03.3C5H6N
80
228.5
«
— 22
18.8
AgNOs.aCsHsN
74
230.6
«
— 10
20.03
"
74
225.4
H
0
22.34
«
80
230.4
«
+ 10
27.21
<(
87
237.1
H
20
33.64
"
90
241.9
"
30
40.86
"
100
253-8
M
40
53.52
«
no
271.4
*
Fusion-point data for mixtures of AgNOa + T1NO3 are given by van Eyk (1905).
SILVER NITRITE AgNO2.
SOLUBILITY IN WATER.
(Creighton and Ward, 1915.)
O
10
15
Cms. AgN02
per Liter.
1-55
2. 2O
2-75
2O
25
30
Cms. AgNOj
per Liter.
3-40
4.14
5
40
50
60
Gms. AgNOj
per Liter.
7-15
9-95
13-63
The determinations by Abegg and Pick (1906) are slightly higher than the
above at temperatures below 20°. Single determinations agreeing well with
the above are given by Ley and Schaefer (1906), and by von Niementowski and
von Roszkowski (1897).
SOLUBILITY IN
Mols, per Liter.
AQUEOUS SOLUTIONS OF SILVER NITRATE AT 18°.
(Naumann and Rucker, 1905.)
Grams per Liter. Mols. per^ Liter Grams per Liter.
AgNO3.
o.oooo
0-00258
0-00517
0.01033
AgNO2.
0.02067
0.01975
0.01900
0.01689
AgN03.
o.ooo
0-439
0.878
I-756
AgN02.
3.184
3.042
2 .926
2 .6ol
AgN03.
0.02067
0.04134
0.08268
AgN02.
0-01435
o. 01168
0-00961
AgN03-
3-512
7.024
14.048
AgN02.
2.201
1-799
1.480
SILVER NITRITE 620
SOLUBILITY OF SILVER NITRITE IN AQUEOUS SOLUTIONS OF SILVER NITRATE
AND OF POTASSIUM NITRITE AT 25°.
(Creighton and Ward, 1915.)
In Aqueous AgNO3. In Aqueous KNO2.
Mols. AgNOj, Dissolved AgNO2 per Liter. Mols. KNO2. Dissolved AgNO2 per Liter.
per Liter. Mols. = Cms. per Liter. Mols. Cms.
o 0.0269 4-135 o 0.0269 4-135
0.00258 0.0260 3-991 0.00258 0.0259 3-974
0.00588 0.0244 3-735 0.00588 0.0249 3.820
0.01177 0.0224 3.432 0.01177 0.0232 3-56o
0.02355 0.0192 2.943 0.02355 0.0203 3-ii9
0.04710 0.0164 2.498 0.04710 0.0181 2.765
Additional determinations of the solubility of silver nitrite in aqueous silver
nitrate solutions at 25° are given by Abegg and Pick (1905).
One liter aqueous 0.02 n NaNO2 dissolves 3.185 gms. AgNO2 at 25°.,
" " " 0.20 n " " 3.016 "
" " " o.2onNaNO3 " 4.956 "
(Ley and Schaefer, 1906; see also p. 660.)
ioo gms. H2O sat. with both salts contain 10.9 gms. AgNO2 + 78.3 gms.
Sr(NO2)i at 14°. (Oswald, 1912, 1914.)
ioo gms. acetonitrile dissolve about 23 gms. AgNO2 at ord. temp, and about
40 gms. at the boiling-point (8l.6°). (Scholl and Steinkopf, 1906.)
SILVER OXALATE Ag2C2O4.
One liter H2O dissolves 0.0378 gm. Ag2C2O4 at 21°, see Note, p. 608.
(Whitby, 1910.)
One liter H2O dissolves 0.0416 gm. Ag2C2O4 at 25°. Conductivity method.
(Schafer, 1905.)
One liter H2O dissolves 0.0265 gm. Ag2C2O4 at 9.72°, 0.034 Sm- at 18.5° and
0.043 gm. at 26.9°. (Kohlrausch, 1908.)
SOLUBILITY OF SILVER OXALATE IN AQUEOUS NITRIC ACID AT 25°.
(Hill and Simmons, 1909.)
Normal-
Per cent
3 t
Gms.
Normal-
Per cent
J -.£
Gms.
ity of
Aq. HNO3.
Cone,
of HNO3.
«25 OI
Sat. Sol.
Ag2C204.
per Liter.
ity of
Aq. HN03.
Cone,
of HNO3.
026 O*
Sat. Sol.
Ag,CA
per Liter .
0.2517
1-574
1.0080
1-345
4.017
22.37
I.I4I5
17.11
0.5025
3-II7
I.OI86
2.189
5-564
29.84
1.1996
29.96
0.9806
6.017
1-0339
3-720
5.83
31.085
I.2I62
33-88
1.040
11.476
I . 0647
7.170
SILVER OXIDE Ag2O.
One liter of H2O dissolves 0.021 gm. at 20°, and 0.025 gm« at 25°.
(Noyes and Kohr; Bottger; Abegg and Cox.)
One liter H2O'dissolves 0.0215 gm. Ag2O at 20°. (See Note, p. 608.) (Whitby, 1910.)
SOLUBILITY OF SILVER OXIDE IN WATER.
(Rebiere, 1915.)
Gm. Mols. Ag2O per Liter. Gms. Ag2O per Liter.
Method of Preparation of the Sample. S_±I . — . ,_ ~i£r — >
At 25 . At 50 . At 25°. At 50 .
By action of NaOH on AgNO3 2.I6.IQ-4 2.97.IQ-4 0.050 0.0691
By action of Ba(OH)2 on AgNOs 2.23.IO"4 s.OQ.icr4 0.0519 0.0719
By action of KOH on AgCl 2.32.10-* 3.55.IQ-4 0.0538 0.0825
By action of KOH on Ag2COj 2 . 95 . lo"4 3 . 89 . lo"4 o . 0680 o . 0904
SOLUBILITY OF SILVER OXIDE IN AQUEOUS AMMONIA AT 25°.
(Whitney and Melcher, 1903.)
Mols. NH3 Gm. Atoms Ag Mols. NH3 Gm. Atoms Ag Mols. NH3 Gm. Atoms Ag
(Total) per Liter. per Liter. (Total) per Liter. per Liter. (Total) per Liter. per Liter.
0.220 0.0658 0.733 0.224 I-I47 0.343
0.469 0.134 0.876 0.257 1.498 0.454
©•.684 O.2O5 0.915 0.276 1.522 0.470
621
SILVER OXIDE
SOLUBILITY OF SILVER OXIDE IN AQUEOUS SOLUTIONS OF ETHYL AMINE AND
OF METHYL AMINE AT 18°.
(Euler, 1903.)
In Aqueous Ethyl Amine. In Aqueous Methyl Amine.
Normality of Normality of Normality of Normality of
Aq. Amine. Dissolved Ag. Aq. Amine. Dissolved Ag.
O.IOO 0.0322 O.IOO O.O22I
0.50 0.160 0.500 0.118
I O-3I4 I O.228
SILVER PERMANGANATE AgMnO,.
100 gms. cold water dissolve 0.92 gm.: hot water dissolves more.
(Mitscherlich, 1832.)
SILVER PHOSPHATE Ag3PO4.
One liter of water dissolves 0.00644 gm. at 20°.
SILVER PROPIONATE C2H5COOAg.
SOLUBILITY IN WATER.
(Raupenstrauch, 1885; Arrhenius, 1893; Goldschmidt, 1898.)
t o ' Gms. C3H5O2Ag to Gms. C3H5O2Ag t<,
per Liter. per Liter.
O 5.12 20 8.36(8.48) 50
10 6.78 25 9.06 70
18.2 8. 36 (A) 30 9.93(9.70) 80
(Bottger, 1903.)
Gms. C3HBO2Ag
per Liter.
13-35
17.64
20.30
SOLUBILITY OF SILVER PROPIONATE IN AQUEOUS SOLUTIONS OF:
(Arrhenius.)
Silver Nitrate at 19.7°.
Mols. per Liter. Gms. per Liter.
Sodium Propionate at 18.2°.
Mols. per Liter. Gms. per Liter.
AgNO3.
C3H502Ag.
AgN03. C3H502Ag.
C3H5O2Na.
C3H6O2Ag.
C3H502Na.
C3H502Ag.
O
0
,0471
O
8.519
O
O,
,0462
0
8.362
0.0133
0.
0415
2
,289 7.511
0.
0167
0
0393
I.
607
7.II4
0.0267
0.
0379
4
,577 6.86
0.
0333
0,
0345
3-
215
6.244
0.0533
0.
0307
9
059 5-556
O.
0667
0.
0258
6.
429
4.670
O.IOO
0.
0222
16,
997 4-019
0.
1333
0.
0191
12.
859
3.456
0.
2667
0.
0131
25.
7l8
2.371
O.
5000
0.
OIOI
48.
77
1.828
SILVER SALICYLATE C6H4.OH.COOAg 1,2.
One liter of aqueous solution contains 0.95 gm. at 23°.
(Holleman,5i893.)
SILVER SUCCINATE C4H4O4Ag2.
100 gms. H2O dissolve 0.0176 gm. at 18°, and 0.0199 Sm- at 25°-
(Partheil and HUbner, 1903.)
SILVER SULFATE Ag2SO4.
O
IO
20
25
Gms. Ag2SO4 per
100 Gms. Sat. Sol.
0-57
0.69
0.79
0.834
SOLUBILITY IN WATER.
(Barre, 1911.)
. „ Gms. Ag2SO4 per
1 * 100 Gms. Sat. Sol.
0.88
30
40
50
60
0.97
1.05
I.I4
70
80
00
100
Gms. Ag2SO4 per
100 Gms. Sat. Sol.
I. 21
1.28
1-34
1-39
The result at 25° is the average of the very accurate and closely agreeing
determinations of Hill and Simmons (1909), Rothmund (1910) and Harkins
(191 1 ). Earlier determinations, differing somewhat from the above, are given by
Euler (1904), Wright and Thompson (1884), Wentzel ( ) and Drucker (1901).
SILVER SULFATE
622
SOLUBILITY OF SILVER SULFATE IN AQUEOUS SOLUTIONS OF AMMONIUM
SULFATE.
(Barre, 1911.)
Results at 33°.
Gms. per 100 Gms.
Sat. Sol.
Results at 51°.
Gms. per 100 Gms.
Sat. Sol.
Results at 75°.
Gms. per 100 Gms,
Sat. Sol.
Results at 100°.
Gms. per 100 Gms.
Sat. Sol.
(NH4)2S04. I
8.85
15.90
22.22
27.25
30.80
35-88
43.22
^g2SO4.
.101
•331
.500
.585
.619
.627
.600
•557
8.90*
16.27
22.43
32.10
35-38
39-03
42.37
45-05
Ag2S04."
1.362
1.680
1.887
2.o6l
2.095
2 .082
2-055
2.026
(NH4)2S04.
8.80
I5-23
22.30
28.25
32
35-82
4I.l6
46.46
Ag2so;.
1.758
2.155
2.490
2.734
2.823
2.889
2.929
2.902
(NH4)2S04.
9.23
15
22.01
27
34.90
38.70
44-15
47.63
Ag2so4:
2.221
2.626
3-075
3-325
3-663
3-772
^867
A series of determinations at 16.5° is also given.
SOLUBILITY OF SILVER SULFATE IN AQUEOUS NITRIC ACID AT 25°.
(Hill and Simmons, 1909.)
Normality
01 Aq.
HNO3.
L-onc. 01 Aq.
HN03.
Sat. Sol.
per Liter.
OI Aq.
HNO3.
^onc. 01 Aq
HN03.
' Sat. Sol.
per Liter.
0
0
I
.0054
8-35
4
.209
23-33
I
.1956
73.212
1.0046
6
•154
I
.O6l
34.086
5
•564
29.84
I
.2456
84 . 609
2.0452
12
.005
I
.1069
49-OIO
8
.487
42.37
I
.3326
94.671
4.017 22.37 1.1871 71.166 10.034 48.77 1.3676 90.806
SOLUBILITY OF SILVER SULFATE IN AQUEOUS SOLUTIONS OF ACIDS AND
SALTS AT 25°.
(Swan, 1899.)
Acid or
Salt.
Gm. Equiv. Gms. Dissolved
per Liter. Ag2SO4 per Liter.
HNO3
0
8.41
"
0.01589
9-33
tt
0.03178
10.18
((
0.06357
11.83
KHS04
0.05264
8.13
tt
0.10526
8.07
Acid or
Salt.
Gm. Equiv. Gms. Dissolved
per Liter. Ag2SO4 per Liter.
H2SO,
O
8.41
u
0.02902
8-55
u
0.05802
8.68
K
O.IO526
8.86
K2SO4
O.O27I8
7-93
tt
0.05434
7.68
SOLUBILITY OF SILVER SULFATE IN AQUEOUS SOLUTIONS OF SALTS AT 25°.
(Harkins, 1911.)
Gm. Eauiv. j
Gms.
Gm. Eauiv.
j *r
Gms.
Salt.
A. **»•
Ag2SO4 per
Liter.
Salt.
Salt
per Liter.
"25 ul
Sat. Sol. *
Ag2S04
per Liter.
KNO3
o
. . .
8-344
AgN03
0.
09961
I
0137
2
.644
u
0
024914
.0072
8.996
K2SO4
O.
025024
i
0064
7
.899
u
0
049774
.0092
9.531
tt
0.
050044
i
0079
7
.694
tt
o
09987
.0034
10.435
tt
0.
IOO
x
0112
7
•49
Mg(N03)2
0
024764
.0073
9.267
"
0.
20003
I
Ol8o
7
.531
"
0
049595
.0094
10.029
MgS04
o.
020022
X
.0061
8
.140
lf
0
09946
•0133
".334
"
o.
050069
X
.0079
7
.941
AgN03
0
024961
.0065
6.095
tt
0.
IOOO4
X
.0105
7
.740
"
0.
04986
.0084
4.487
tt
0.
20005
X
0164
7
• 733
One liter of aqueous solution in contact with a mixture of silver sulfate and
silver acetate contains 3.95 gms. Ag2SO4 + 8.30 gms. CH3COOAg at 17°. Sp. Gr.
of solution = 1.0094. (Euler, 1904.)
623
SILVER SULFATE
SOLUBILITY OF SILVER SULFATE AT 25° IN AQUEOUS SOLUTIONS OF:
(Drucker, 1901.)
Sulfuric Acid.
Mols. per Liter. Cms. per Liter.
Potassium Sulfate.
Mols. per Liter. Cms, per Liter.
Ag2S04.
H2SO4.
Ag2S04.
H2so4:
'Ag2S04.
K2S<V
Ag2S04.
K2so4:
O.O26O
O.O2
8. ii
0.98
0.0246
O.O2
7.67
1.74
0.0264
0.04
8.23
1.96
0.0236
O.O4
7.36
3-49
0.0271
O.IO
8-45
4.90
0.0231
O.IO
7.20
8.72
0.0275
O.2O
8.58
9.81
0.0232
O.2O
7.24
17.44
SOLUBILITY OF SILVER SULFATE IN AQUEOUS POTASSIUM SULFATE SOLUTIONS.
(Barre, 1911.)
Results at 33°. Results at 51°. Results at 75°.
Results at 100°.
Gms. per 100 Gms.
Sat. Sol.
Gms. per 100 Gms.
Sat. Sol.
Gms. per 100 Gins.
Sat. Sol.
Gms. per 100 Gms.
Sat. Sol.
K2S04.
3.22
5-62
8-37
10.41
11.80
Ag2S04.
0.863
0.940
1.046
I.II7
I.I77
'K2S04.
3-20
5-6l
8.40
10.55
I3.l6
14-37
Ag2S04.
1.023
I.I27
1.247
1.340
1.450
1.524
'K2S04.
3-12
5-73
8-43
10-55
13-17
17.06
Ag2SO4.
1.273
1.406
1-554
1.665
i. 806
2.021
K2S04.
3-23
5.60
8-45
11.30
I5.07
18.58
Ag2S04.
1.488
I.675
1.890
2.H5
2.410
2.677
Results at 14.5° are also given.
SOLUBILITY OF SILVER SULFATE IN AQUEOUS SODIUM SULFATE SOLUTIONS.
(Barre, 1910, 1911.)
Results at 33°.
Gms. per 100 Gms.
Sat. Sol.
Results at 51°.
Gms. per 100 Gms.
Sat. Sol.
Results at 75°.
Gms. per 100 Gms.
Sat. Sol.
Results at iood.
Gms. per too Gms.
Sat. Sol.
Na2S04.
Ag2S04.
Na2SO4.
Ag2SO4.
Na2S04.
Ag2SO4.
Na2S04. Ag2S04.
0.25
0.861
0.25
1.032
O.20
I.2I5
0.50
•341
0.98
0.816
1.02
0-995
0.98
I. 210
1. 01
.363
2.OI
0.832
1.90
I.OI7
1.96
1.238
1.94
.418
3
0.867
2.92
1-053
2.98
1.296
3-02
•494
5-34
0.972
5-40
I-I73
5-37
1.458
5-33
.651
10.05
1.150
IO. II
1-379
9.81
1.697
IO.I5 2.OI2
20.09
1.448
20.25
1-705
19.98
2.075
25-45 2.351
29-55
1-570
29.23
1.802
29.66
2.138
34.72 2.012
39-44
1.462
39-30
1.540
38.94
1.603
38.63 1.687
46.976
0.932
44.46
0.882
41.36
I.I56
40.16 I.I58
Results at 14.5° and at 18° are also given.
SOLUBILITY IN SILVER SULFATE IN AQUEOUS 0.5 n SOLUTIONS OF VARIOUS
COMPOUNDS AT 25°.
(Rothmund, 1910.)
Aq. 0.5 n
Gms.
Dissolved
Aq. 0.5 »
Gms.
Dissolved
Aq. 0.5 n
Gms.
Dissolved
Solution of:
Ag2SO<
per Liter.
Solution of:
Ag2S04
per Liter.
Solution of:
Ag2S04
per Liter.
Methyl Alcohol
7-
764
Glycerol
8
.202
Acetonitrile
16.
37
Ethyl Alcohol
7-
109
Mannitol
9
.262
Glycocol
13
50
Propyl Alcohol
6
798
Grape Sugar
8
.418
Acetic Acid
7
857
AmyPAlc. (tert.)
6
36
Urea
9
.448
Phenol
ii
,81
Acetone
6
.86
Dimethylpyrone
6
.736
Chloral
7,
,266
Ether
6
424
Urethan
7
.078
Methylal
6
393
Formaldehyde
7
078
Formamide
8
.42
Methyl Acetate
6
61
Glycol
8.
076
Acetamide
7
•794
Fusion-point data for Ag2SO4 + Na2SO4 are given by Nacken (1907).
SILVER SULFIDE 624
SILVER SULFIDE Ag2S.
One liter H2O dissolves about 4.10-" gm. atoms Ag as sulfide at about 18°.
(Bernfeld, 1898.)
One liter H2O dissolves 0.55. lO"6 gm. mols. = 0.0001363 gm. Ag2S at 18°.
(Weigel, 1907.)
Fusion-point data for AgaS -f- ZnS are given by Friedrich (1908).
SILVER SULFONATES
SOLUBILITY IN WATER AT 20°.
(Sandquist, 1912.)
<?iilfnnati» Cms. Sulfonate"'
per 100 Gms. H2O.
Silver .2 Phenanthrene Monosulfonate] o.ooo
" -3 " 0.20
" .10 0.52
SILVER TARTRATE C4H4O6Ag2.
100 gms. H2O dissolve 0.2012 gm. C^OeAgjj at 18°, and 0.2031 gm. at 25°.
(Partheil and Hiibner, 1903.)
SILVER THIOCYANATE AgSCN.
SOLUBILITY IN WATER.
t°. Gm. AgSCN per Liter. Authority.
20 O.OOOI4 (Bottger, 1903.)
21 0.00025 (Whitby, 1910. See'Note, p. 608.)
25 O . OOOI 7 (Kuster and Thiel, 1903.)
25 O . OOO2 (Abegg and Cox, 1903.)
100 0.0064 (Bottger, 1906.)
Additional data for the solubility of AgSCN in water are given by Kirschner
(1912.)
SOLUBILITY OF SILVER THIOCYANATE IN AQUEOUS POTASSIUM THIOCYANATE
AT 25°. (Hellwig, 1900.)
Mols. KSCN Mols. AgSCN Gms. AgSCN Mols. KSCN Mols. AgSCN Gms. AgSCN
per Liter. per Liter. per Liter. per Liter. per Liter. per Liter.
0.573 0.0124 2.06 1. 12 0.0975 16.18
0.626 0.0168 2.08 1.20 0.120 iQ-93
1. 066 0.0850 14.01 1.25 0.134 22.34
One liter of aqueous 3 n AgNO3 dissolves 0.0432 gm. AgSCN at 25.2°. (Hellwig, 1900.)
SILVER VALERATES AgC6H9O2.
Normal Valerate, CH3(CH2)3.COOAg. Iso Valerate, CH3.CH(CH3)2CH2COOAg.
SOLUBILITY OF EACH SEPARATELY IN WATER.
(Fiirth, 1888; Sedlitzky, 1887.)
Gms. per 100 Gms. H2O. Gms. per 100 Gms. HaO. •
t0' Normal V. Is^T. t0' Normal V. Iso V. "
o 0.229 °-I77 50 Q-474 0.360
10 0.259 0.211 60 0.552 0.401
20 0.300 0-246 70 0.636 0.443
30 0.349 0.283 80 ... 0.486
40 0.408 0.321
loo gms. H2O dissolve 0.73 gm. silver valerate at 20°. (Markwald, 1899.)
loo cc. sat. aq. solution contains 0.71 gm. dextro silver valerate at 15°.
(Taverne, 1900.)
625
SILVER VALERATE
SOLUBILITY OF SILVER VALERATE IN AQUEOUS SOLUTIONS OF SILVER
ACETATE, SILVER NITRATE AND OF SODIUM VALERATE.
(Arrhenius, 1893.)
In
Silver Acetate at 17.8°.
In Silver Nitrate at 16.5°.
IMols.
per Liter.
Gms. per Liter.
Mols. per Liter.
Gms.
per Liter.
C2H302Ag.
0
0.0067
C6H902Ag.
0.0094
O.0070
C^HiAAg. CBH9O2Ag.
o 1.96
I . 13 I . 46
AgN03. C5H902Ag.
o 0.0094
0.0067 0.0068
AgNO3.
0
I.I4
C6H902Ag.
1.96
1.42
0.0135
O.027O
0.0505
0.0057
0.0037
0.00265
2.27 I.I9
4.54 0.77
8.48 0.55
0.0133 0.0051
0.0267 O.003I
O.IOOO O.OOI2
2.29
4.58
17.
1.07
0.65
0.25
In Sodium Valerate at 18.6°.
Mols.
per Liter.
Gms. per Liter.
C2H302Na.
O
0.0175
0.0349
0.0698
CBH902Ag.
0.0095
0.0047
0.0030
O.OOlS
C2H,02Na.
0
2.17
4-32
8.65
CBH902Ag.
1.986
0.982
0.627
0.376
0.1395
0.0015
17. 31
0.313
SILVER VANADATE Ag,V4Qii.
One liter of aqueous solution contains 0.047 gm. at 14°, and 0.073 gm. at iOo°
(Carnelly, 1873.
SODIUM Na.
SOLUBILITY IN LIQUID AMMONIA.
(Ruff and Geisel, 1906.)
t".
105
70
50
Mols. NH3 Required
to Dissolve i Gm.
Atom Na.
4.98
5.20
5-39
t°.
-30
0
+ 22
Mols. NH3 Required
to Dissolve i Gm.
Atom Na.
5-52
5-87
6.14
SOLUBILITY OF SODIUM IN MELTED SODIUM HYDROXIDE.
(von Hevesy, 1909.)
t°. 480° 600° 610° 670° 760°
Gms. Na per zoo Gms. NaOH 25.3 10.1 9.9 9.5 7.9
800°
6.9
Saturation could not be reached at temperatures below 480°. The saturated
mixtures were cooled by plunging the container in water and the solidified con-
tents analyzed.
SOLUBILITY OF SODIUM IN MELTED SODIUM HYDROXIDE CONTAINING OTHER
METALS AT 480°.
(von Hevesy, 1909.)
'Added
Metal.
Gms. Added
Metal per 100
Gms. NaOH.
Gms. Dissolved
Na per 100
Gms. Solvent.
Added
Metal.
Gms.
Metal
Gms.
Added
per too
NaOH.
Gms. Dissolved
Na per 100
Gms. Solvent.
Thallium
5
.40
23.13
Cadmium
2
.87
24-34
M
8
•30
23.54
u
3
.l6
24.29
M
12
.42
21.29
Gold
6
•03
23.92
It
31
•37
20.91
"
8
.22
23.39
Zinc
30
•37
25.38
SODAMMONIUM Na2(NH3)2.
100 gms. liquid ammonia dissolve 60.5 gms. Na2(NH3)a at —23°, 56.4 gms. at
0°, 56 gms. at +5° and 55 gms. at 9°. (Joannis, 1906.)
SODIUM ACETATE 626
SODIUM ACETATE CH3COONa.3H2O.
Cms.
t°.
CH3COONa
per 100
Cms. H2O.
— 10
19
-18
30-4
— 10
33
o
36.3
+10
40.8
20
46.5
30
54-5
40
65.5
50
83
58
138
0
119
IO
121
SOLUBILITY IN WATER.
(Green, 1968.)
Solid Phase.
Ice
CH3COONa.3H2O
Cms.
t°.
CH3COONa
per 100
Cms. H2O.
20
123.5
30
126
40
129.5
50
134
60
139-5
70
146
80
153
90
161
100
170
no
180
120
191
123 b. pt.
193
Solid Phase.
CH3COONa (unstable)
CH3COONa (unstable)
" Results differing somewhat from the above are given by Kohler (1897) ; Enklaar
(1901) and Schiavor (1902).
SOLUBILITY OF SODIUM ACETATE IN AQUEOUS SOLUTIONS OF ACETIC ACID AT
VARIOUS TEMPERATURES.
(Dunningham, 1912.)
Results at o°. Results at 15°. Results at 30°. Results at 75°.
Gms. per 100 Gms.
Sat. Solution.
Gms. per too Gms.
Sat. Solution.
Gms. per roo Gms.
Sat. Solution.
Gms. per 100 Gms.
Sat. Solution.
Solid Phase
in
.NazO. (CH3CQ)2O.
29-34
(CH3CO)20
0-15
. Na2O.
35-31
26.25
(CH3CO)2C
0.77
8.92
>. Na-,0.
44-45
32.47
22.30
17.85
11.05
7.63
0.44
(CH3CO)20. Each Case.
0.76 CHjCOONa
5.03
36.69
. . . CH3COONa.3H20
" +1.1
43 • 06 i.i
65.71
8i.49
98.35
" +1.2
... 1.2
«
««
«
el
«
24.12
14.46
9-72
9-77
9.04
2.04
8.55
41.23
43-94
25-94
15-49
n-45
11.25
10.33
10.22
9.l6
4
12
23
34
39
39
49
.19
.01
•54
-56
.08
•73
-32
25-
18.
13-
13-
13-
7-
98
09
53
24
14
64
9
13
21
33
32
65
.06
.62
.88
.05
.90
.07
8.96
8.72
7-83
6.19
4.02
1.05
0.42
44.80
45.10
50.03
62.44
79.29
92.29
97-51
8.56
7.06
5-95
4.84
2.87
i. 02
0.79
.54
61
70
77
86
95
98
•34
•63
-55
.60
.61
-87
.09
7-
6.
5-
3.
2.
I.
67
33
61
52
78
94
27
66
69
72
77
83
86
94
-42
.68
-85
.76
•92
-73
.78
i.i = CH3COONa.CH3COOH. 1.2 = CH3COONa.2CH3COOH.
Additional data for 5°, 20°, 45° and 60° are also given.
Similar data for 30° are given by Dukelski (1909), and for 20° by Abe (191 1-12).
One determination at 25°, expressed in terms of volume of solution, is given by
Herz (1911-12). Two determinations at 10° similarly expressed, are given by
Enklaar (1901).
Data for the freezing-point of mixtures of sodium acetate and acetic acid are
given by Vasilev (1909).
627
SODIUM ACETATE
SOLUBILITY OF SODIUM ACETATE IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Gms. CHjjCOO-
Wt. Per cent
QHsOH in
Solvent.
•, n( Gms. CH3COO-
SfttSoL NGm?2srri°°
0
1.209
55-7
IO
1. 160
53
20
i.i35
49-8
30
1.108
46.5
40
1.072
42
50
1.038
37
Wt. Per cent
, *
QHsOH in
Solvent.
Sat5 Sol.
60
0.990
70
0.942
80
0.882
90
0.838
95
0.828
IOO
0.823
30.4
22.8
13
6.7
6.1
7-3
The solid phase in contact with the solution was CH3COONa.3H2O in all
cases.
ioo gms. absolute alcohol dissolve 7.49 gms. CH3COONa.3H2O at room temp.
(Bodtker, 1897.)
SOLUBILITY OF SODIUM ACETATE IN AQUEOUS ALCOHOL:
At Different Temperatures.
(Schiavor, 1902.)
At 1 8°.
(Gerardin, 1865.)
Wt.
Per cent
Alcohol.
Gms. CH3COONa
per ioo Gms.
Aq. Alcohol.
5-2
38
9.8
35-9
23
29.8
29
27-5
38
23-5
45
20.4
59
14.6
86
3-9
91
2.1
t°.
Degree
of
Alcohol.
Gms. per too Gms. Alcohol.
CH3COONa.
CH3COONa.3H2O.
8
98.4
2.08
3-45
12
98.4
2.12
3-51
19
98.4
2-33
3-86
II
90
2.O7
3-42
13
90
2.13
3-52
15
63
I3-46
22.32
18
63
13.88
23.03
21
63
14.65
24.30
23
40
28.50
47.27
ioo gms. H2O dissolve 237.6 gms. sugar + 57.3 gms. CH3COONa, or 100
gms. of the saturated solution contain 58.93 gms. sugar + 14.44 gms. CH3COONa
at 3 1. 25°. (Kohler, 1897.)
ioo cc. anhydrous hydrazine dissolve 6 gms. sodium acetate at room temp.
(Welsh and Broderson, 1915.)
ioo gms. propyl alcohol dissolve 0.97 gm. sodium acetate. (Schlamp, 1894.)
SODIUM SulfoANTIMONATE Na3SbS4.9H2O.
•o.i
•0.65
•0.9
•1.26
•1-45
Gms.
NajSbS4per
too Gms.
Sat. Sol.
0-5
4
5-7
7.8
9.2
Solid
Phase.
Ice
SOLUBILITY
IN WATER
(Donk,
1908.)
Gms.
to Na3SbS4 per Solid
ioo Gms. Phase.
Sat. Sol.
— I
0
.75 II. 2
II. 8
Ice
Na3SbS4.9H2O
15
30
38
19-3
27.1
32
it
r.
49.6
59-6
69.6
79-5
Gms.
Na3SbS4 per Solid
ioo Gms. Phase.
Sat. Sol.
38.9 Na3SbS4.9H20
45
50.7
57-1
SOLUBILITY OF SODIUM SULFOANTIMONATE IN AQUEOUS SOLUTIONS OF SODIUM
HYDROXIDE AT 30°.
(Donk, 1908.)
Gms. per ioo Gms. Sat. Sol.
Na3SbS4.
27.1
NaOH.
0
ooua rnase.
Na3SbS4.9H2O
13
5-9
9.9
24.8
«
10.5
32.9
•
Na3SbS4.
NaOH.
* ooua rnase.
16.4
42.6
Na2SbS4.9H,O
17.7
47.2
"+NaOH.H2O
9.1
49-5
NaOH.H2O
0
54.3
SODIUM SulfoANTIMONATE
628
SOLUBILITY OF SODIUM SULFOANTIMONATE IN AQUEOUS SOLUTIONS OF SODIUM
THIOSULFATE.
(Donk, 1908.)
Results at o°.
Gms. per 100 Gms. Sat. Sol.
' Na3SbS4.
Solid Phase.
ii. 8
4.4
0.8
O.I
o
o
o
4-9
14.6
27-3
33-6
33-6
Na3SbS4.9H20
Na8S20J.SHiO
Results at 30°.
Na3SbS*.
19.9
12-5
Na2S203. '
7-7
16.4
ooiia rnase.
Na3SbS4.9H20
4-2
37-7
"
I
43-8
"
I
47
"
I
47.8
" +Na2S203.5H20
0
45-8
Na2S203.SH20
SOLUBILITY OF SODIUM SULFOANTIMONATE IN AQUEOUS ETHYL ALCOHOL.
(Donk, 1908.)
Results at 30°.
Cms. per 100 Gms. Sat. Sol.
Results at 65°.
Gms. per 100 Gms. Sat. Sol.
Results at o°.
Gms. per 100 Gms. Sat. Sol.
N&sSbS^ CjHsOri.
ii. 8 o
8.2 3.7
3.2 12.7
0.9 29
o 60.8
* Two liquid layers separate between these concentrations of alcohol. The composition of several
of these conjoined layers is as follows:
Na3SbS4.
C2H5OH.
Na3SbS4.
C2HBOH. '
19-3
5
47-9
0
14.6
10.3
39-3
4-7
6.4
24.8
36.5
8*
1.2
46
4.1
54.i*
0
76.2
o
81
Gms. per 100 Gms. Alcoholic Layer.
Na3SbS4.
4.1
10.2
I4.I
Gms. per 100 Gms. Aqueous Layer.
54-1
40.4
33-5
o
Na3SbS4.
36.5
27.8
24.1
18
C2HBOH.
8
14.3
18.8
27.2
The solid phase in contact with each of the above solutions is Na3SbS4.9H2O.
SOLUBILITY OF SODIUM SULFOANTIMONATE IN AQUEOUS METHYL ALCOHOL.
(Donk, 1908.)
Results at oc
' Na3SbS4.
CH3OH."
OUilU JTllitSC.
8.6
3-4
Na3SbS4.9H26
2.8
15-5
"
2.1
23.1
«
0-3
50.3
"
O.I
57
«
0.05
81.7
"
O.2
92
«
2
95-9
M
Results at 30°.
Gms. per 100 Gms. Sat. Sol.
Na3SbS4.
CH3OH.
27.1
12.8
O
18.1
5.8
O.I
O.I
33-i
65.7
84.2
1.2
91.2
3-9
94
Solid Phase.
Na3SbS4.9H2O
SODIUM ARSENATE Na3AsO4.i2H2O.
100 gms. aqueous solution contain 21.1 gms. Na3AsO4.i2H2O (= 10.4 gms.
Na8AsO4) at 17°. Sp. Gr. of solution = 1.1186. (Schiff, 1860.)
100 gms. glycerol dissolve 50 gms. sodium arsenate at 15.5°. (Ossendowski, 1907.)
629
SODIUM ARSENATES
EQUILIBRIUM IN THE SYSTEM SODIUM OXIDE, ARSENIC TRIOXIDE, WATER AT 25°.
(Schreinemakers and de Boat, 1917.)
Solid Phase.
AS20V
N&£>.
ouiiu niiibc.
As-A.
Na2O.
2.019
0
AsA
3I-05
21.82 ]
14.45
2-45
"
±29
±22.7
24.42
4-23
"
21.92
24.04
37-73
6.46
"
17-50
25.64
58.54
9.60
"
14.26
29.16
±73
±12
" +NaAs02
14-63
30.24
63.01
12.73
NaAs02
19.32
32.04
57-90
13.24
"
15-53
33-57
48.05
14.27
M
10.49
36.21
36.32
18.74
"
6-59
39-39
±34
±21.1
" +Na4As205.9H20
5-ii
39-69
32.24
21.6
Na4As2O6.9H2O
o
41.2
+NaioAs4On.26H,O
Na10As4O11.26H2O
+NaOH.H2O
NaOH.H2O
SODIUM Hydrogen ARSENATE Na2HAsO4.i2H2O.
SOLUBILITY IN WATER.
(Average curve from results of Schiff, 1860; Tilden, 1884; Greenish and Smith, 1901.)
Cms. Na2HAsO4
per 100 Gms. H2O.
O
10
IS
7-3
15-5
20.50* =
= 1.1765)
20
25
30
Gms. Na2HAsO4
per 100 Gms. H2O.
26.5
33
37
40
60
80
Gms.
per loo Gms.
47
65
85
SODIUM Diethyl BARBITURATE Na(C8HnO8N2).
SOLUBILITY IN WATER.
(Puckner and Hilpert, 1909.)
16.87
Gms. Salt per 100 Gms. Sat. Sol.
SODIUM BENZOATE C6H5COONa.
5°
6.08
25°
17.18
32-50
SOLUBILITY IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Wt. Per cent
C2H5OH in
Solvent.
O
IO
20
30
40
50
SODIUM (Tetra) BORATE Na2B4O7.ioH2O (Borax).
SOLUBILITY IN WATER.
(Horn and Van Wagener, 1903.)
1
#25 OI
3ms. C6H5COONa
per 100 Gms.
Sat. Sol.
Wt. Per cent
C2H5OH in
Solvent.
&c of G
Sat. Sol.
ms. C6H5COONa
per loo Gms.
E Sat. Sol.
-155
36
60
0-975
21.3
.132
35-3
70
0.927
15-4
.110
33-7
80
0.877
8.8
.086
90
0.831
2.8
•055
28.9
95
0.812
1.3
.020
25-6
100
0-795
0.6
t°.
0-5
IO
21.5
30
37-5
45
Gms.
per roo Gms.
H20.
i!6
2.8
3-9
5-6
8.1
5o
54
II
57
Gms. Na2B4O/7
per too Gms.
H20.
10.5
13-3
14.2
II
60
62
65
70
80
oo
IOO
Gms. NajB4O7
per 100 Gms.
H20.
19.4
20.3
22
20.7
22
21.9
24-4
31-5
41
52-5
Tr. temp., Na2B4O7.ioH2O->Na2B4O7.5H2O, approximately 62°.
^16.5° of sat. sol. = I.O2O. (Greenish and Smith, 1901.)
ioo gms. H2O dissolve 3.33 gms. Na2B4O7 at 25°, determined by refractometer.
(Osaka, 1903-08.)
SODIUM BORATES
630
SOLUBILITY OF SODIUM BORAXES IN WATER AT 30°.
(Dukelski, 1906, complete references given.)
Cms, per 100 Gms. Solution. Gms. per 100 Gms. Residue.
' NaA
B203.
Na20. B203. '
42.0
NaOH.H2O
41-37
5.10
43.54 4.19
38.85
5-55
37-20 II. 1 8 Na2O .B2O3.4H2O
34-44
3-73
33.52 I0.8o
29-39
2.51
29.63 io.ii "
26.13
2-75
27.85 15.21
23.00
3.82
24.91 II. 60
16.61
13.69
21.29 20.64
21.58
4-63
24.52 1 9 . 04 Na2O .B2O3.4H2O +|Na2O.B2O3.8H2O
20.58
4.69
21. 6 1 16.59 NajsO .B2O3.8H2O
I5-32
6.21
19.70 17.84
12.39
9.12
18.05 18.17
8.85
10.49
11.72 2O.62 Na20 .2B2O3.ioH2O
5.81
6.94
IO.82 21.31
1.88
2.41
7-31 J5-5o
1-38
5-i6
7.16 17.44
2.02
7-79
6.24 16.38
4.08
17.20
8 . 96 29 . 20 Na2O.2B2O3.ioH2O + Na2O.5B2O8.ioH2G
3-79
15.84
5 . 68 28.19 Na20.sB203.ioH20
2.26
12.14
5-21 29.19
1.99
11.84
5 . 74 39 . 66 Na2O.2B2O3.ioH2O + B(OH)3
1.86
ii. 18
1. 06 28.78 B(OH)3
0.64
6. ii
0.31 31.19
3-54
... "
EQUILIBRIUM IN THE SYSTEM SODIUM OXIDE, BORIC OXIDE, WATER AT
60°.
(Sborgi and Mecacci, 1915, 1916.)
Gms. per 100 Gms.
Gms. per 100 Gms.
Sat.
Sol.
Solid Phase. Sat. Sol. Solid Phase.
NajO.
B203.
NaaO. B2O3.
49-25
O
NaOH.H2O 19.29 22.78 Na20.B2O3.4H2O
48.44
0.81
20.30 25.50
49.28
i-53
" +2Na2O.B2O3.H2O 22.21 32.17 " +Na2O.2B2O3.s
H2C
47.38
2. 24
2Na2O.B2O3.H2O 19-43 27.09 Na20.2B2O3.sH2O
44-74
3.78
16.13 23.05 «
42-94*
5.67
" +Na2O.B2O3.H2O 13-51 IQ.IO
40.14
5-41
Na2O.B2O3.H2O 1 1- 58 16.62 "
38.70
5.56
6.95 11.50 "
35.76
6.29
5.65 14.89 «
34-93
6.80
" 6.84 20.40 "
31-88
9.85
" (unstable) 8.42 28.05 "
29-56
11.83
" 11.29 41.47 " +Na20.5B203.ioH20
28.07
14.65
8.29 33.57 Na20.SB203.ioH20
33-12
7-47
" +NajO.B2O3.4H2O 6.29 28.77
28.64
6.51
Na20.B2O3.4H2O 3-22 21.94
22.06
10.29
3-40 22.59 " +H3BO,
18.72
J7-33
1.39 13.92 H3B03
18.32
19.17
o 7.39
SODIUM BORAXES 631
SOLUBILITY OF SODIUM BORAXES IN SEVERAL SOLVENTS.
Borate.
Sodium borate
Sodium Biborate
Solvent. f.
Alcohol (d= 0.941) 15.5
Glycerol 15.5
80
Trichlorethylene 15
gS*. Authori*-
2 . 48 (u. s. P. vm.)
60.3 <u. s. p. vm.)
100 (u. s. P. vni.)
o. on (Wester and Bruins, 1914.)
Gms. NaBrO3 per 100 Gms. H20
Fusion-point data for mixtures of NaBO2+NaPO3 and NaBO2+Na2SiO3 are
C" ren by Van Klooster (1910-11). Results for Na2B4O7+Na4P2C)7 are given by
Chatelier (1894).
SODIUM BROMATE NaBrO3.
SOLUBILITY IN WATER.
(Kremers, i8ss-s6a.)
0° 20° 40° 60° 80° 100°
27.5 34-5 50-2 62.5 75.7 90.9
Sp. Gr. of saturated solution at 19.5° = 1.231. (Gerlach.)
100 cc. anhydrous hydrazine dissolve I gm. NaBrO3 with decomposition.
(Welsh and Broderson, 1915.)
SODIUM BROMIDE NaBr.2H2O.
SOLUBILITY IN WATER.
So!id Phase. V. £%*&& Solid Pb**.
Ice 50 53.7 (4) NaBr.2H2O
" +NaBr.SH2C, 50.7 53-9(5
NaBr.sH2O+NaBr.2H2O 80 54-2(4
NaBr.2H2O
to
Gms. NaBr per
.
100 Gms. Sat. Sol.
— IO.I
20.8 (i)
-28
40.3 (2)
-23.5
41.2 (3)
— 20
41.8(4)
— 10
42.9 (4)
0
44.3 (4)
+16.4°
47 (8)*
20
47 -5 (4)
30
49-4(7)
40
5i-4(4)
50
50.
80
100
no
140
180
210
230
+NaBr
NaBr
54-8 (4)
55-1 (4)
56.5(6)
59-5(6)
60.9 (6)
62 (6)
1-523).
(i) Rudorff (1862); (2) Guthrie (1875); (3) Panfiloff (1893); (4) de Coppet (1883); (5) Richards
and Churchill (1899); (6) Etard (1894); (7) Cocheret (1911); (8) Greenish (1900).
SOLUBILITY OF SODIUM BROMIDE IN AQUEOUS SOLUTIONS OF SODIUM
HYDROXIDE AT 17°.
(Ditte, 1897.)
Gms. per 100 Gms.
Gms. per too Gms. H2O.
Gms. per 100 Gms. H2O.
NaOH.
NaBr.
NaOH.
NaBr.
NaOH.
NaBr.
0-0
9I.38
17.17
63.06
28.43
48.00
3.26
79.86
19.12
62 .51
36.61
38.4I
9.24
68.85
22-35
59.60
46.96
29-37
13-43
64.90
24.74
55-03
54-52
24.76
SOLUBILITY OF SODIUM BROMIDE IN AQUEOUS ETHYL ALCOHOL AT 30°.
(Cocheret, 1911.)
CjHjOH.
NaBr.
ouuu riiiise.
O
49-4
NaBr.2H2O
11.79
31.78
43-22
54.59
42.9
32.12
26.79
20.83
"
Gms. per too Gms. Sat. Sol.
'C2H6OH. NaBr. '
65.51 16.08
72.36 13.41
76.92 I2.O3
87.35 7-44
97 . 08 3 . 01
Solid Phase.
NaBr.2H2O
" +NaBr
NaBr
SODIUM BROMIDE
632
SOLUBILITY OF SODIUM BROMIDE IN ALCOHOLIC SOLUTIONS.
(Rohland, 1898-05; de Bruyn, 1892; Eder, 1876.)
Alcohol.
Concentration
of Aq. Alcohol.
t°.
Cms. NaBr
per 100 Gms.
Alcohol.
Methyl Alcohol
^i5=o-799
room temp.
21-7 (R.)
Ethyl
d15=o.8io
tt
7.14
Propyl
d15=o.8i6
«
2.01
Ethyl
90% by vol.
?
4.0 (hydrated NaBr)
Methyl "
Absolute
19-5
17.35 (de Bruyn.)
Ethyl
it
15
6.3 (NaBr2H20) (Eder.)
Ethyl Ether
:c
15
0.08
^ A sat. solution of NaBr in CH3OH contains 0.9 gin. NaBr per 100 gms. solu-
tion at the critical temperature. (Centnerszwer, 1910.)
loo cc. of ethyl alcohol of d = 0.8327 dissolve 7.37 gms. NaBr at 16.4°, du of
Sat. sol. = 0.889. (Greenish, 1900.)
ioo gms. propyl alcohol dissolve 2.05 gms. NaBr at ord. temp. (Schlamp, 1894.)
SOLUBILITY OF SODIUM BROMIDE IN MIXTURES OF ALCOHOLS AT 25°.
(Herz and Kuhn, 1908).
In CH3OH + C2H6OH.
Per cent Gms.
CH3OH A* of NaBr per
in Sat. Sol. ioo cc.
In CH3OH + C8HrOH.
Per cent Gms.
CjH7OH <*25 of NaBr per
in Sat. Sol. too cc.
In C2H6OH + C3H7OH.
Per cent Gms.
CSH7OH ^25 of NaBr pei
e in Sat. Sol. ioo cc.
Mixture.
Sat. Sol.
Mixture.
Sat. Sol.
Mixture.
Sat. Sol.
O
0.
8189
2-93
0
0.9238
14.40
0
0.8189
2-93
4-37
0.
8265
3.65
II.
n
0.9048
12-43
8.
i
0.8147
2.49
10.4
0.
8273
4.04
23-
8
0.8887
10.53
17-
85
O.8l45
2.47
41.02
0.
8593
7,24
65-
2
0.8390
4.42
56.
6
0.8107
1.90
80.69
0.
9079
12.51
91.
8
0.8153
1.47
88.
6
0.8116
I. II
84.77
0.
9104
12.86
93-
75
0.8144
1.26
91.
2
0.8083
0.83
91.25
0.
9235
14.32
IOO
0.8093
0.74
95-
2
o . 8090
0.82
roo
0.
9238
14.40
IOO
0.8093
0.74
SOLUBILITY OF SODIUM BROMIDE IN ACETAMIDE AT VARIOUS TEMPERATURES.
(Menschutkin, 1908.)
Gms. per ioo Gms.
Sat. Sol.
N -
Solid Phase.
82*
8o
78
76
74
72
80
CONHj
6
II- 5
16.3
2O. 2
23
25
27
... CHjCONH,
2.8 «
5-36 "
7.6 «
9.4 "
10.7 «
1 1. 6 "+NaBr.2CH3CONH2
12.6 NaBr.aCHjCONHj
* M. pt. f Tr. pt.
•\
*"• s
3ms. per ioo Gms.
Sat. Sol.
Solid Phase.
aBr.2CHr
CONH2 =
NaBr.
90
29.4
13-7
NaBr.2CH3CONH,
IOO
32.2
IS
"
no
35-3
16.4
«
120
38-7
18
"
130
42.6
19.8
«
i3St
45-3
21. I
" +NaBr
155
46.4
21.6
NaBr
175
47-5
22. I
"
t Eutec
ioo gms. 95% formic acid dissolve 22.3 gms. NaBr at 18.5°.
(Aschan, 1913.)
ioo cc. anhydrous hydrazine dissolve 37 gms. NaBr at room temp.
(Welsh and Broderson, 1915.)
FUSION-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES.
NaBr + NaCl
NaBr + Nal
NaBr + NaF.
NaBr + NaOH
NaBr + NaNO2.
NaBr + Na2SO,
(Amadori,
(Amadori,
(Ruff and Plato, 1903.)
(Scarpa, 1915-)
(Meneghini, 1912.)
(Ruff and Plato, 1903.)
; Ruff and Plato, 1903.)
633
SODIUM CACODTLATE (CH3)2AsO.ONa.
SODIUM CACODYLATE
100 gms. H2O dissolve about 200 gms. of the salt at I5°-2O°. (Squire and Caines, 1905.)
loo cc. 90% alcohol dissolve about 100 gms. of the salt at I5°-2O°. "
SODIUM CAMPHORATIS
SOLUBILITY IN AQUEOUS d CAMPHORIC ACID SOLUTIONS AT i3.5°-i6°.
(Jungfleisch and Landrieu, 1914.)
Gms. per 100 Gms.
Sat. Sol. Solid Phase.
C10H1(A. C10HM04Na2.
O.62I O Ci0H16O4
2.03 4.19 "
2.87 8.32
3.03 10.05 "
2.97 7.80
2.87 9.06
2.94 10.46
2.68 14.99
2-64 17.53
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
2-74
2.63
1 +C10H16O4Na.2Ci0H16O4.2H2O 2.29
C10H1604Na.2C10H1604-2H20 2.17
1. 06
0.88
O
CioH1804. CwH1404Na2.
2 . 87 25 . 62 C10H1604Na.2C10H1804.2H^)
2.89 27.41
30.69
32.75
40. 10 CMH16O4Na.H2O (or iH20)
40-54
47.04
49 . 60 C10H14O4Na2.3H20
50.2
CioHi6O4 = Camphoric acid. CioHi6O4Na.2CioHi6O4.2H2O = Monosodium d tri-
camphorate. Ci0Hi5O4Na.H2O = Monosodium d camphorate. CioHuC^Na-^HjO
= Disodium d camphorate (neutral).
(The mixtures were kept in a cellar at a nearly constant temperature and
shaken from time to time. Additional determinations at i7°-23° are also given.)
SODIUM CARBONATE Na2CO3.ioH2o.
SOLUBILITY IN WATER.
(Wells and McAdam, Jr., 1907; Mulder, below 27° and above 44°.)
r.
Gms.
NajCOa per
loo Gms. H2O.
O
7
5
9.5
10
15
12-5
16.4
20
27.84
21-5
34-20
29-33
37-40
30.35
40.12
3L45
32.06
43-25
32.15
33-10
30.35
32.86
43.50 -
46.28
Solid Phase.
Gms.
+Na2C03.7H20
+Na2C03.H20
t°.
Na.COa p
100 Gms. I
34-76
48.98
35-62
50.08
35.50
. . .
29.86
50.53
31.80
50.31
35.17
49-63
36.45
49-36
37-91
49.11
41.94
48.51
43-94
47.98
60
46.4
80
45.8
TOO
45-5
105
45-2
Solid Phase.
NajCO,.7H2O
NajCOj-HjO
The determinations of Wells and McAdam, Jr., were made with extreme care.
They correct the discrepancies which have so far existed between the solubility
and transition points of the hydrates. Earlier data, which differ more or
less from the above, are given by Lowel, 1851; Reich, 1891; Eppel, 1899 and
Ketner, 1901-02. Single determinations at 15°, 25°, and 30° are given by
Greenish and Smith (1901); Osaka (1910-1911); de Paepe (1911) and Cocheret
(1911).
Sp. Gr. of solution saturated at 17.5°, 1.165 (Hager); at 18°, 1.172 (Kphl-
rausch); at 23°, 1.22 (Schiff); at 30°, 1.342 (Lunge). See also Wegscheider
and Walter, 1905, for Sp. Gr. determinations at other temperatures.
SODIUM CARBONATE
634
EQUILIBRIUM IN THE SYSTEM SODIUM CARBONATE, SODIUM BICARBONATE,
AND WATER AT 25°.
(McCoy and Test, 1911.)
'(Forty grams of NaHCO3 and about 200 cc. of H2O were rotated at 25° until
equilibrium was reached. Small portions of the clear solution were then ana-
lyzed by the Winkler method for carbonate content, and by titration in presence
of methyl orange, for sodium. About 15 gms. of Na2CO3.ioH2O were then added,
and the mixture again rotated until equilibrium was reached, and again analyzed.
This was continued and the following results were obtained.)
Solid Phase.
Na2C03.ioH2O
" +Na2CO3.NaHC03.2H2O
Na2CO3.NaHC03.2H2O
* " +NaHCO3
NaHCO,
Per cent of
Total Na
Present as
Bicarbonate.
Gms. Na
per Liter.
Gms.
Bicarbonate
per Liter.
Gms. Carbonate
per Liter.
O
II9.9
O
276.4
5-92
127.6
27.6
276.3
7-5
120
10
107
12.89
108
50.8
216.6
15
100
20
80
. . .
...
32
60
. . .
. . .
56
40
. . .
. . .
80
30
100
27.02
98.7
O
The following data for this system also at 25°, but given in terms of weight
instead of volume of solution, are reported by de Paepe (1911).
Gms. per 100 Gms. H2O.
NaHCOs'.
O
2.1
4.2
5-7
28.3
27-3
26.5
19.2
Solid Phase.
NaaCCvioHjO
" +NaHC03
NaHCO8
Gms. per 100 Gms. H2O.
NaaCOs. NaHCO3.
12.4 7-3
6.2 9
I 10. 1
Solid Phase.
NaHCO,
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM
BROMIDE AND OF SODIUM IODIDE AT 30°.
(Cocheret, 1911.)
In Aq. NaBr Solutions.
Na2C03.
NaBr. "
27.98
O
NajCO3.ioH2O
27-54
2.41
«
26.72
4.06
««
26.23
6.26
" +Na2C03.7H20
23.40
II
Na2C03.7H2O
22.68
12.22
"
19.86
16.88
"
19-57
16.95
" +Na2C03.H20
i8.ii
19.32
NazCOj.HzO
8-45
33-39
"
6.90
36-13
"
3-04
44-75
"
2.99
45-31
" +NaBr.2H2O
2.60
45-68
NaBr.aH2O
0
49.40
"
In Aq. Nal Solutions.
Na2CO3.
Nal.
26.5
2.4
Na2C03.ioH2O
25-5
4-7
"
24.4
8.6
"
24-3
9-5
" +Na2C03.7H20
23
II .2
Na2C03.7H2O
20.8
14
"
18.7
18.4
"
15-3
25-4
" +Na2CO3.H2O
13-1
29.1
Na2CO3.H2O
10.4
33-3
"
4.2
46
"
2-7
.51
"
0.9
57-6
"
o-3
65.6
" +NaI.2H20
0
65-5
NaI.2H2O
635
SODIUM CARBONATE
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 15°.
(Reich, 1891.)
Gms. per 100 Gms.
H2O.
Gms. NaCl
per
Gms. NajCOj
per 100 Gms.
Gms. per too Gms.
H20.
NaCl.
Na2CO3.io-
H20.
looGms.
Solution.
NaCl
Solution.
NaCl. I
^COfio-
0
61.42
o
16.42
23.70
39-06
4.03
53-86
2.92
14-47
27-93
39-73
8.02
48
5-8o
12.87
31.65
41.44
12. O2
43.78
8.61
11.62
35-46
43-77
16.05
40.96
11-31
10.70
37-23
45-27*
19.82
39.46
I3-7I
10. II
* Both salts in solid phase.
Gms. NaCl Gms. Na-jCOa
per
100 Gms.
Solution.
per 100 Gms.
NaCl
Solution.
15.96
18.26
20.06
21-75
22.46
9.76
9.62
9-73
7-95
10.13
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SODIUM CHLORIDE AT 30°
(Cocheret, 19 n.)
Gms. per 100 Gms. Sat. Sol.
Na2C03.
27.98
27.48
27.12
26.82
25-59
24. 26
22.75
NaCl.
o
0.90
3-33
4-iS
5-17
5-93
10.24
Solid Phase.
Gms. per 100 Gms. Sat. Sol.
+Na2C03.7H20
+Na2CO,.H20
Na2C03.
NaCl.
> ouiiu runsc.
20.72
11.49
NajCOs.HjO
18
14. 12
" +NaCJ
14.81
16.26
NaCl
9.71
18.76
"
5.65
21-94
«
o
26.47
<«
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM NITRATE.
(Kremarm and Zitek, 1909.)
, Gms. per TOO Gms. H2O. ^
t°. c
10
10
IO
24.2
24.2
Ims. per 100 Gms. H2O. ^ __
u. 98*
8-75
o
28.55
26.33
NaNO3.
O
70.48
80.5
0
45.96
" +NaNO3
NaNO3
Na-sCOj.ioHzO
24.2
24.2
24.2
24.2
24.63
21.8
5.96
0
NaNO3.
54-43
62.7
84.45
91-3
Na2C03.7H20
" +NaNO,
NaNO,
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS ETHYL ALCOHOL AT 30°.
(Cocheret, 1911.)
Solid Phase.
Gms. per 100 Gms. Sat. Sol.
' NajCOs. QHfiOH. "
26.61 2.64 NajCOj.ioHjO
26.14 3-41*
Gms. per 100 Gms. Sat. Sol.
Solid Phase.
1.38
0.62
0-53
0.51
44-81*
52.99
55-70
56.56
+Na2C03.7H20
NajCO,.
C;,H6OH.
— » OU11U JTllttSC.
0.40
63.20
Na2CO3.7H2O
O. II
73.06
" +Na2COs.H,0
O.O7
78.19
NajCOj.HjO
0.06
90.95
"
0.03
95.06
" +Na2C03
98.46
NajCO,
* Between these two concentrations, the mixtures separate into two liquid layers.
Results are also given for the solubility of Na2CO3 + NaBr and of Na2CO3
+ NaCl in Aq. C2H6OH at 30°.
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF ETHYL AND OF
PROPYL ALCOHOL AT 20°.
(Linebarger, 1892.)
Wt. Per cent Gms. Na^COa per 100 Gms. Sol.
Alcohol. ' In Ethyl In Propyl. '
28 ... 4-4
38 ... 2.7
44 1-7 1-7
46 1.13 i-S
Wt. Per cent
Alcohol.
48
50
54
62
Gms. NajCOj per 100 Gms. Sol.
In Ethyl.
0.9
0.84
0.80
In Propyl.
i-3
1.2
0.9
0.4
SODIUM CARBONATE 636
SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL.
(Ketner, 1901-02.)
NOTE. — The mixtures were so made that alcoholic and aqueous layers were
formed, and these were brought into equilibrium with the solid phase.
Gms. per 100 Gms. Alcoholic Layer. Gms. per 100 Gms. Aq. Layer.
t°. , * s / * > Solid Phase.
C2H5OH. Na2CO,. H2O. C2HbOH. Na2CO3. H2O.
35 62.9 0.3 36.8 i 32.4 66.6 Na2co3.H2o
40 61 0.4 38.6 1.2 31.9 66.9 "
49 61 0.4 38.6 1.2 31.5 67.3
68 55.8 0.9 43.3 2.3 28.8 68.9
31.2 52.4 0.8 46.8 ... 29.3 ... Na2CO3.7H2O(0)
31.9 54.8 0.7 44.5 1.7 29.8 68.5
32.3 56.1 0.6 43.3 1.5 30.2 68.3
33.2 58.1 0.5 42.4 1.4 ' 31 67.6
27. 7 Crit. sol. ± 14% C2H2OH ± 13% Na2CO., ± 73% H2O
28.2 23.5 7.3 69.2 7.9 18.6 73.5 NajCOj.ioHjO
29 32.7 3.8 63.5 4.3 22.7 73.0
29.7 40 2.1 57.9 2.9 25.5 71.6
30.6 47.8 1.2 51 2.3 27.8 69.9 "
SOLUBILITY OF Na2CO3.ioH2O IN DILUTE ALCOHOL AT 21°.
(Ketner.)
Gms. per 100 Gms. Solution. Gms. per 100 Gms. Solution.
Na,COj. QHSOH. H2O. N^COj. QH5OH. H2O.
18.5 O 81.5 1.2 39.2 59.6
12.7 6.2 81.1 0.2 58.2 41.6
6.9 15.3 77.8 o.i 67.1 32.8
3.2 26.1 70.7 0.06 73.3 26.64
Isotherms showing the compositions of the conjugated liquids at 28.2°, 29.7°
and 40° are also given.
EQUILIBRIUM IN THE SYSTEM SODIUM CARBONATE, NORMAL PROPYL ALCOHOL
AND WATER AT 20°.
(Frankforter and Temple, 1915.)
(Note. In this paper the results for the binodal curve are reported in terms of
gms. per 100 gms. solvent (water -f- alcohol), instead of gms. per 100 gms. of the
homogeneous liquid (sodium carbonate + water + alcohol.)
Gms. per 100 Gms. Alcohol + Water. Gms. per 100 Gms. Alcohol + Water.
Na^CO,. Alcohol. Water. Na^COj. Alcohol. Water.
16.568 3.409 96.591 J-99o 31-537 68.463
15.363 4.472 95-528 1.338 40.796 59-204
11.696 6.595 93-405 0.930 46.933 53-067
8.415 9-176 90.824 0.567 53-875 46.125
6.669 n. 221 88.779 0.298 59-507 40.493
4.138 15.785 84.215 0.160 63.568 36.432
2.878 21.099 78.901 0.109 75-159 24.841
For results on the system sodium carbonate, allyl alcohol, water at 20° see
last table, p. 647.
100 gms. glycerol (du = 1.256) dissolve 98.3 gms. Na2CO3 at i5°-i6°.
(Ossendowski, 1907.)
loo gms. saturated solution in glycol contain 3.28-3.4 gms. sodium carbonate.
(de Coninck, 1905.)
100 gms. H2O dissolve 229.2 gms. sugar + 24.4 gms. Na2CO3, or 100 gms. sat.
aq. solution contain 64.73 gms. sugar -f- 6. 89 gms. Na2CO3 at 31.25°. (Kohler, 1897.)
637
SODIUM CARBONATE
EQUILIBRIUM IN THE SYSTEM SODIUM CARBONATE, PYRIDINE, WATER.
(Limbosch, 1909.)
Very pure materials were used. The boiling-point (cor.) of the pyridine was
115°-! 15.07°. Increasing amounts of this pyridine were added to aqueous
solutions of sodium carbonate contained in glass tubes. After the tubes were
sealed they were placed in a bath and the temperature noted at which the liquid
mixture passed from a homogeneous to an opalescent condition. During the
observation, the contents of the tubes were stirred by means of pieces of iron,
moved with the aid of a magnet on the outside of the tube.
Per cent
of
Per cent
of
t° of Sat.
Per cent
of
Per cent
of
Per cent
t° of Sat. of
Per cent
of
t° oi bat.
Pyridine.
NajCOs.
Pyridine.
Na,CO3.
Pyridine.
O.I29
66.2
12
2.
5o
50
199
6.12
23-
5
1 2O
0.129
66.4
25
2.
5o
53-3
197
6.12
25.
5
132
O.I29
67.7
36
2.
5o
59-4
173
6.12
28.
4
152
0.129
69.2
44
2.
50
69.2
123
6.99
13-
8
54.2(40.5)
0.129
73-5
53
2.
5o
73-8
1 10
6.99
15-
4
81
d7)
o. 129
74.8
2.
5o
74-8
*
6.99
19.
5
117
0.129
76.1
25. s(— 64)
3-
49
30-3
-0-5
6.99
22.
7
142
o. 129
77-8
ii (-59)
3-
49
32.6
39
6.99
25-
i
158
I.OI
47.6
17
3-
49
34-3
86.5
6.99
27.
6
169
I .OI
49-9
36
3-
49
36.7
107
6.99
32.
6
180+
I.OI
51-2
55
3-
49
37-4
123
9.36
8.
50
64
(26)
I.OI
52.2
72
3-
49
42.5
194
9.36
9
78
(18)
I.OI
56-1
107
3-
49
69.6
167
9.36
ii.
4
106.5
I.OI
60.6
in
3-
49
71.2
*
9.36
13-
8
127
I.OI
66.8
no
5-
23
23-3
63(27
.5) 9.36
16.
3
148
I.OI
75-i
86.5
S-
23
23-7
70(20
.5) 9.36
20.
i
169
I.OI
76.9
71
5-
23
24.6
79
9.36
25
180+
I.OI
78.1
*
5-
23
26.2
96
9-36
50
180+
2.50
36.3
22
5-
23
28.7
in
18.1
2.
12
48
(18)
2.50
37-9
53-25
§•
23
32.5
155
18.1
2.
25
66
2.50
39-2
74-5
5-
23
36.6
196
18.1
2,
70
79
2.50
40
94
5-
23
37-2
200+
I*, i
4
20
108
2.50
43-6
147
5-
23
55-4
*
18.1
5
,40
126
2.50
47.6
185
18.1
6
80
155
* Precipitate of NajCOs. Results in parentheses show lower temperatures of saturation.
Fusion-point data for Na2CO3 + NaCl are given by Le Chatelie 0*1894) and
Sackur (1911-12). Results for Na2CO3 + NazSO* are given by Le Chatelier
(1894), Sackur (1911-12) and by Amadori (1912). Results for Na2CO3 + KC1
are given by Sackur (1911-12).
SODIUM (Bi) CARBONATE NaHCO3.
SOLUBILITY IN WATER.
(Dibbits, 1874; Fedotieff, 1904.)
o
10
20
25
Cms. NaHCOs per 100 Cms.
Water.
6.9
8.15
9.6
10.35
Solution.
6.5
7.5
8.8
9-4
30
40
50
60
Cms. NaHCO per 100 Cms.
Water. Solution.
ii. i 10
12.7 11.3
14.45 I2-6
16.4 13.8
100 gms. H2O dissolve 9.03 gm. NaHCO3 at 15°, di6 = 1.061.
(Greenish and Smith, 1901.)
100 gms. alcohol of 0.941 Sp. Gr. dissolve 1.2 gms. NaHCO3 at 15.5°
100 gms. glycerol dissolve 8 gms. NaHCO3 at 15.5°. (Ossendowski, 1907.)
SODIUM (Bi) CARBONATE
638
SOLUBILITY OF SODIUM BICARBONATE IN AQUEOUS AMMONIUM BICARBONATE
SOLUTIONS SATURATED WITH CO2.
(Fedotieff, 1904.)
.0 Wt. of i cc. !
* - Solution.
Ylols.per IDC
>o Gms.H20
NHtHCOs.
NaHCO3".
o 1.072
i-39
0.58
tt
o.o
0.82
g
.056
O-O
1.05
it
.061
0.29
o-95
tt
.065
0.56
0.89
It
•073
1. 08
0.79
It
.090
2.16
0.71
30
o.o
1.65
tt
2.91
0.83
Grams per 1000 Gms. H2O-
'NH4HCO3. NaHCO3. '
109.4
O.O
0-0
23.0
44.0
85-7
170.6
o.o
230
48.2
69.0
88.0
80.0
74.6
66.7
59-2
138.6
70.0
SOLUBILITY OF SODIUM BICARBONATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE SATURATED WITH CO2.
(Fedotieff; see also Reich, 1891.)
0
Wt. of i cc.
Mols. per icx
DO Gms.H2O.
Grams per i<
XXD Gms. H2<
Solution.
NaCl.
NaHCO3.
NaCl.
NaHCO3.
o
0-0
0.82
0-0
69.0
u
1. 208
6.0
O.O9
35° -1
7-7
15
I .056
o.o
1.05
O-O
88.0
1.063
0.52
0.82
30.2
68.6
t(
1.073
1.03
0.64
60. 1
53-6
It
1.096
2. II
0.41
123 .1
34-8
It
I.I27
3-20
0.28
187.2
23.0
u
1.158
4-39
O.I9
256.9
16.1
tt
1.203
6.06
O.I2
354-6
IO.Q
30
1.066
o.o
I .31
o.o
no. 2
tt
1.079
1.02
0.87
59-9
72.8
tt
i .100
2.08
0.56
121.9
47-3
tt
i .127
3.18
0.38
186.3
32-0
tl
1.156
4-38
0.27
256.0
22.3
tt
1.199
6.12
0.17
358-1
13-9
45
1.077
o.o
I.6S
o.o
138.6
tt
i. 086
1.04
1. 12
60.7
94.0
"
1.115
2.65
O.62
155-2
52.0
"
i -127
3-24
0.52
189.4
43-4
u
i .155
4-38
o-37
256.1
30-7
tt
1.198
6.18
0.23
361-5
19-5
100 gms. alcohol of 0.941 Sp. Gr. dissolve 5.55 gms. sodium sulfocarbonate at
15-5°.
SOLUBILITY OF SODIUM BICARBONATE IN AQUEOUS SODIUM NITRATE
SOLUTIONS.
(Fedotieff and Koltunoff, 1914.)
o
15
15
15
Sp. Gr. of
Sat. Sol.
I-356
1.183
1.285
1-377
Gms. per 100 Gms. H2O.
'NaNO3. NaHCO3.'
72.74 1.41
29.06 3.40
54.56 2.l6
83.20 1.57
95.14 I. 80
639 SODIUM CHLORATE
SODIUM CHLORATE NaC103.
SOLUBILITY IN WATER.
(Carlson, 1910; Le Blanc and Schmandt, 1911; Osaka, 1903-08.)
,„ dof
* • Sat. Sol.
Gms. NaClOs per to
zoo Gms. EkO.
dof
Sat. Sol.
Gms. NaClO3 per
loo Gms. H2O.
-15
I
.380
72-
40
I
.472
126
(i 15 LeB.&S.)
0
I
.389
79
(80 LeB.&S.)
50
140
(126
10
89
(87
60
I
.514
155
15
I
.419
95
(91 "
70
172
20
I
.430
IOI
(95-7 "
80
I
•559
I89
25
I
•44
1 06
(101 O.)
IOO
I
.604
230
30
JI3
(105 Le B. & S.)
122 (b. pt.)
I
.654
286
The earlier data of Kremers (1856) lie between the values of Carlson and of
Le Blanc and Schmandt.
SOLUBILITY OF SODIUM CHLORATE IN AQUEOUS SODIUM CHLORIDE SOLUTIONS
AT 20°.
(Winteler, 1900.)
Sp. Gr. of
Gms. per Liter.
Sp. Gr. of
Gms. per Liter.
Solutions.
Nad.
NaClO3.
Solutions.
NaCl.
NaClO,.
1.426
5
668
I
.365
175
393
I.4I9
25
638
I
•345
2OO
338
I.4I2
5o
599
j
319
225
271
1.405
75
559
I
,289
250
197
1.398
IOO
522
I,
,256
275
1 20
1.389
125
484
j
•235
290
78
1-379
150
442
I
.217
300
55
100 gms. H2O dissolve 24.4 gms. NaCl + 50.75 gms. NaClO3 at 12°.
loogms. H2O dissolve 1 1 .5 gms. NaCl + 249.6 gms. NaClO3at 122°. (Schlosing, 1871.)
SOLUBILITY OF SODIUM CHLORATE IN AQUEOUS ETHYL ALCOHOL.
(Carlson, 1910.)
Gms. NaClO3 per Liter of Sat. Sol. in Aqueous Alcohol of:
If .
50 Per cent.
75 Per cent
90 Per cent.
20
3I3-3
II0.8
16.1
40
60
70
321.8
326.8
133-5
155-8
161.3
22.9
29
gms. alcohol of 77 Wt. per cent dissolve 2.9 gms. NaClO3 at 16°. (Wittstein.)
gms. alcohol dissolve i gm. NaClO3 at 25°, and 2.5 gms. at b. pt.
IOO
IOO
100 gms. glycerol dissolve 20 gms. NaClOs at 15.5°. (Ossendowski, 1907.)
100 cc, anhydrous hydrazine dissolve 66 gms. NaClOs at room temperature.
(Welsh and Broderson, 1915.)
SODIUM PerCHLORATE NaClO4.H2O.
SOLUBILITY IN WATER.
(Carlson, 1910)
is
50
143
dot
Sat. Solution
Gms. NaClO4
per TOO cc.
Sat. Solution.
Solid Phase.
1.666
107.6
NaClCvHjO
I-73I
1.789
123.4
141.4
NaCIO.
SODIUM CHLORIDE 640
SODIUM CHLORIDE NaCl.
SOLUBILITY IN WATER.
(Mulder; de Coppet, r883,'Andrae, 1884; Raupenstrauch, 1885; above 100°, Tilden and Shenstone,
1884; Berkeley, 1904; Etard, 1894, gives irregular results.)
to Cms. NaCl per Gms^NaCl
AO Gms. NaCl per
Gms. NaCl
looGms-HaO. jooTsoL
100 Gms. H2O.
per
ioo g. Sol.
o 35-7* 35-63t 26.28!
70 37.8* 37-5if
27-27t
10 35-8 35.69 26.29
80 38.4 38.00
27-54
20 36.0 35.82 26.37
90 39-o 38-52t
27.80
25 36-12 35-92 26-43
ioo 39.8 39-I2J
28.12
30 36-3 36-°3 26.49
118 39.8
28.46
40 36.6 36.32 26.65
140 42 . 1
29.63
50 37.0 36.67 26.83
160 43-6
30-37
60 37.3 37-06 27.04
180 44-9
30.98
* M.; de C. t
A. * B.
The original, very carefully determined
figures of Berkeley, are as
follows.
f0 d of Gms. NaCl per
Sat. Sol. loo Gms. H2O.
+o doi
Sat. Sol.
Gms. NaCl per
ioo Gms. H2O.
0.35 1.2090 35.75
6l.70 1.1823
37-28
t5.20 1.2020 35.84
75.65 1.1764
37-82
30.05 1.1956 36.20
90.50 I.I7OI
38.53
45.40 1.1891 36.60
107 b. pt. 1.1631
39.65
ioo gms. H2O dissolve 35.99 gms. NaCl at 30°. (Cocheret, 1911.)
SOLUBILITY OF SODIUM CHLORIDE IN WATER, DETERMINED BY THE FREEZING-
POINT METHOD.
(Matignon,
Gms. NaCl
t°. per ioo Gms. Solid Phase.
t°.
Gms. NaCl
per ioo Gms. Solid Phase.
H2O.
H20.
0.4
0.69
Ice (Raoult)
-12.7
20
Ice
0.8
1-37
" (Biltz)
-16.66
25
"
2.86
4.9
" (Kahlenberg)
-21.3
30.7
" +NaCl.2H2O
3-42
5.85
" (Raoult)
-14
32.5
NaCl.2H2O (de Coppet)
6.6
II
"
— 12.25
32.9
" (Matignon)
9.25
15
"
— 6.25
34-22
" (de Coppet)
Data for the influence of pressure on the solubility of sodium chloride in water
are given by v. Stackelberg (1896); Cohen, Inouye, and Euwen (1910) and by
Sill (1916).
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS SIMULTANEOUSLY
SATURATED WITH OTHER SALTS.
The various papers of J. H. van't Hoff and collaborators, on this subject, have
been collected by H. Precht and E. Cohn in a volume entitled " Untersuchungen
iiber die Bildungsverhaltnisse die Ozeanischen Salzablagerungen," Leipzig, 1912,
p. 374- By far the larger part of the new data in these papers are for solutions
simultaneously saturated with three or more salts and are, therefore, beyond the
limits of complexity of mixture, set for the present volume. The various systems
are described in detail and diagrams are given. A table summarizing much of
the data (van't Hoff (1905)) is given on the following page.
641 SODIUM CHLORIDE
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS SIMULTANEOUSLY
SATURATED WITH OTHER SALTS AT 25°.
(van't Hoff, 1905.)
Mols. per 1000 Mols. HjO.
Solution Saturated with Respect to NaCl and:
K2C12. MgCl2. MgSO4. .
1 0.5 105 ...... MgCl2.6H2O -f Carnallite
2 5.5 70. 5 ...... KC1 + Carnallite
44 20 ... ... 4.5 " -|- Glaserite
44 10.5 ...... 14-5 Na2SO4+ "
46 ... ... 16.5 3.0 " + Astrakanite
26 ... 7 34 ... MgSO4.7H20 + Astrakanite
4 «... 67.5 12 ... " +MgS04.6H20
2.5 ... 79 9.5 ... Kieserite +
i ... 101 5 ... " + MgCl2.6H2O
23 14 21.5 14 ... KC1 + Glaserite + Schonite
19.5 14.5 25.5 14.5 ... " + Leonite -f-
9.5 9.5 47 14.5 ... " + " -f Kainite
2.5 6 68 5 ... " + CarnaUite + "
i i 85.5 8 ... Kieserite + Carnallite + Kainite
42 8 ... 16 6 Na2SO4 + Glaserite -f Astrakanite
27. 5 10. 5 16.5 18.5 ... Schonite + Glaserite + Astrakanite
22 10. 5 23 19 ... Leonite + Glaserite + Astrakanite
10.5 7.5 42 19 ... + MgSO4.7H2O 4- Astrakanite
9 7-5 45 19.5 ... "4- " 4- Kainite
3-5 4 65.5 i3 ... MgS04.6H20+" 4- "
1.5 2 77 10 ... MgSO4.6H2O + Kieserite + "
i 0.5 100 5 ... CarnaUite + MgCl2.6H20 + "
1 0.5 105 ...... MgCl2.6H2O + Carnallite
2 5-5 70.5 ...... KC1 +
CaCl2.
i ... 51.5 90. 5 ... MgCl2.6H2O + Tachhydrite
i ii ... 146 ... KC1+ CaCl2.6H2O
i ... 35.5 121.5 ... Tachhydrite + CaCl2.6H2O
i 1.5 50.5 90.5 ... MgCl2.6H2O+Tachhydrite+Carnallite
i 9.5 5 141 . 5 ... CaCl2.6H2O + KC1 + CarnaUite
i 2 34.5 121.5 ... CaCl2.6H2O+Tachhydrite+ Carnallite
Carnallite = KMgCl3.6H2O, Glaserite = K3Na(SO4)2, Astrakanite = Na2Mg-
(SO4)2.4H2O, Kieserite = MgSO4.H2O, Leonite = MgK2(SO4)2.4H2O, Schonite =
MgK2(SO4)2.6H2O, Kainite = MgSO4.KC1.3H2O.
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM
CHLORIDE.
(Fedotieff, 1904.)
f o Wt. of i cc. Mols. per 1000 Gms. H2O. Gms. per 1000 Gms. H2O.
Solution. ' NH4C1. NaCl. ' 'NI^Cl. N^O?
o ... o 6.09 o 356.3
.185 2.73 4.89 146.1 286.4
15 .200 o 6.12 o 357-6
191 1.07 5-58 57-3 326.4
183 2.22 5.13 II8.9 300
176 3-48 4.64 186.4 271.6
175 3.72 4.55 198.8 266.8
30 ... o 6.16 o 360.3
1.166 4.77 4.26 255.4 249
45 ••• o 6.24 o 365
6.02 4 322.1 233.9
SODIUM CHLORIDE
642
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS AMMONIA AT 30°,
(Hempel and Tedesco, 1911.)
Gms. per 1000 cc. Sat. Sol.
Sat" Sol. ' NH3. NaCl. "
I.I735 29.535 293.38
1.1656 40-655 292.5
1.160 47.26 289.7
I.I494 60.78 286.5
Data for equilibrium in the system sodium chloride, arsenic trioxide, water, at
30°, are given by Schreinemakers and deBaat (1915).
dsoof
Gms. per 1000 cc. Sat. Sol.
Sat. Sol.
NH3. NaCl. '
I . 1406
72.07 283.38
I-I395
72.715 283.06
I.I30I
81.855 277.49
I.I205
97.49 270.57
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
CHLORIC ACID.
(Engel, 1888; Enklaar, 1901.)
AtO°. (Engel.)
Gms. per Liter.
Mg. Mols. per 10 cc.
HCl. NaCl.
Sp. Gr. of
Solution.
0.0
1.0
1.85
9.28
30.75
54-7
53 •$
52.2
48-5
44-0
37-9
23-5
6.1
207
204
202
196
185
173
i .141
i .119
HCl.
NaCl".
o.o
32.0
0.365
0.674
30-5
1.859
28.4
3-38
25-7
5-49
22.2
ii .20
13-7
20.54
3-6
At I0°-I0.5°. (Enklaar.)
Mols. per Liter. Grams per Liter.
HCl.
NaCl."
o.o
6. ii
0.27
5-77
o-35
5-67
0-43
5-59
o-57
5-43
0.72
5-28
2.60
3-42
2.80
3-i8
3.31
2-74
Results at o° and at 25°.
(Armstrong and Eyre, 1910-11.)
Gms. HCl
per Liter
of Solvent.
O
9.II
18.22
36.45
182.25
Gms. NaCl per 100 Gms. Sat. Sol.
At o°. At 25°.
26.35 26.52(^25=1.2018)
25.30 25.45(^25=1.1970)
24.15 25.42(^25=1.1915)
21.93 22.34(^25=1.1822)
7.04(^25=1-1238)
NaCl.
35-77
33-76
33-19
32.71
3i-77
30.89
20.01
19.04
16.03
Results at 25°. Results at 30°.
(Herz, 1911-12.) (Schreinemakers, 1909-10.)
Gms. per 100 Gms.jSat. Sol.
HCl.
0.0
9.84
12.76
15.68
20.78
26.06
94-77
102. 1
I2O.6
Mols. per Liter.
HCl.
0.607
1.032
1.590
2.II7
3.283
NaCl.
4.850
4.467
3.782
3-297
2-343
HCl.
o
6.93
12.50
17-35
35-60
NaCl.
26.47
16.16
9.35
4.52
O.II
Results at 30°. (Masson, 1911.)
Gm. Mols. per Liter. ^ of Gms. Mols. per Liter.
Sat. Sol. '~HCL NaCl. *
1.1427 3.052 2.463
1.1289 4.152 1.628
1.1188 5-950 0.630
1.1258 7.205 0.268
In the case of the results of Masson equilibrium was approached from above and
the solutions were kept in a thermostat and shaken occasionally during 2-6 days.
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS CALCIUM CHLORIDE SOLUTIONS
AT 25°.
(Mills and Wells, 1918.)
Sat. Sol.
HCl.
NaCl.
I. 20l8
O
5.400
I . 1906
0-4575
4-932
I . l8oi
0.969
I.I633
1.786
3.589
I.I5I2
2.412
2.978
Gms. per 100 Gms. Sat. Sol.
Sat. Sol.
CaCl2.
NaCl. '
I.2O7
I. 103
25.30
I. 210
2.l6o
24.32
1.209
3.220
23-37
1.216
5-451
20.43
I.22O
7.398
19.17
^ Of Gms. per 100 Gms. Sat. Sol.
Sat. Sol, ' CaCl2. NaCl.
1.225 9-50 17-55
1.233 "-48 I5-9I
1.241 17.77 IO-54
1.257 21 8.05
1.276 24.58 5.63
643
SODIUM CHLORIDE
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS POTASSIUM NITRATE AT 25.
(Ritzel, 1911.)
Cms, per 100 cc. Sat. Sol. Cms, per 100 cc. Sat. Sol.
KNO3. NaCl. KNO3. NaCl. "
O 31.80 12 30.86
4 32-26 16 30.45
8 1-8 20 30.10
NaCl.
31.80
32-26
31-85
Data for the solubility of NaCl in aqueous MgCl2 solutions are given by Feit
and Przibylla (1909.)
Solvent.
Water
SOLUBILITY OF MIXTURES OF SODIUM CHLORIDE AND OTHER
SALTS IN WATER, ETC.
to Gms. per 100 Gms. Solvent. Authority.
17
25
80
Alcohol (40%) 25
Water 20
25
26.4 NaCl+22.iNH4Cl*
34-5 " + 4-iBaCl2
38.3 « +29-5KN03
38.5 " +41-14 "
39.81 " +168.8 "
I5-78 +13-74 "
30.54 +I3-95
28.90 " +16.12
* Sp. Gr. of solution at 17° = 1.179.
(Karsten.)
(Soch — J. Physic. Ch. 2, 46, '08.)
(Quoted by Euler — Z. physik. Ch.
49, 315. '04-)
SOLUBILITY OF MIXTURES OF SODIUM CHLORIDE AND POTASSIUM SULFATE
IN WATER AT VARIOUS TEMPERATURES.
(Precht and Wittgen, 1882.)
to Grams per 100
Grams H2O. f 0
Grams per 100 Grams
H2O.
NaCl
K2S04
KCl
NaCl
K2S04
KCl
10
33-4
8
.1
3
.2
60
36-4
II
•9
2
•7
20
34-o
8
-9
3
.1
7o
36.6
12
.8
3
.2
30
34-6
9
.6
2
•9
80
36.0
12
•3
5
.1
40
35-2
10
•4
2
.8
9o
35-9
12
4
7
• O
50
35-8
ii
.1
2
.8
100
35-6
12 ,
6
8
.8
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
BICARBONATE SATURATED WITH CO2. (Fedotieff 1904.)
3°
«
1?
Wt. of i cc.
Solution.
I. 208
1.203
1.203
I .196
I.I99
1.189
I.I98
Mols. per 1000 Gms. H2O.
Gms. per 1000 Gms. H2O.
NaHCO3.
NaCl.
0
6.09
0.09
6
O
6.12
O.I2
6.06
0
6.16
0.17
6.12
0
6.24
0.23
6.18
'NaHC03.
NaCl. '
O
356.3
7-7
350-1
0
357-6
IO
354-6
0
360.3
13-9
358.1
0
365
19-5
361.5
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SODIUM HYDROXIDE AT 30°
Gms. per 100 Gms. Sat. Sol.
' Na20. NaCl.
o 26.47
4.47 21.49
12.22 13.62
24.48 4-36
(Schreinemakers, 1909-10, 1910.)
Solid
Phase.
NaCl
NasO.
NaCl. '
OUUU i 11<UC.
29.31
2.40
NaCl
37.85
1. 12
"
41.42
0.97
" +NaOH.H2O
±42
0
NaOH.H2O
SODIUM CHLORIDE
644
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SODIUM HYDROXIDE
SOLUTIONS.
At o° (Engel).
Mg. Mols. per 10 cc.
NajO.
O
4-8
6-73
10.41
14.78
30.50-
37.88
53-25
NaCl.
54-7
49-38
47-21
42.38
39-55
24.95
19.30
9.41
Sp. Gr. of
Solutions.
207
221
225
236
249
295
314
1.362
(Engel; Winteler, 1900.)
Gms. per Liter.
NaOH.
O
38.4
53-8
183.2
118.2
244
303
426
NaCl.
320
288.9
276.2
247.9
23I-4
146
112 .9
55
At 20° (Wintelei
Gms. per Liter. gt
).
>. Gr. of
jluiions.
[.200
NaOH.
10
NaCl. ' S
308 ]
SO
297 1.230
100
253
.250
150
2I3 ]
.270
200
173 3
.290
300
100
112 3
6l
•330
•375
500
640
30 -425
18 1.490
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND VICE VERSA.
(Bodlander, 1891; Nicol, 1891; results at 25° by Soch, 1898.)
NaCl in Aqueous NaNOa.
Results at 15.5° (B.).
NaNO3 in Aqueous NaCl.
Results at 15° (B.).
Sp. Gr. of
Gms. per
ioo cc. Sat.
Solution.
Sp. Gr. of
Gms. per
ioo cc. Sat
. Solution.
Solutions.
NaN03.
H20.
NaCl.
Solutions.
NaCl.
H20.
NaN03.
1.2025
O
88.47
31
.78
I
•3720
0
74.82
62
•38
I-2305
7
•53
87.63
27
.89
I
•3645
4-0
75-69
56
.76
1.2580
13
.24
86.25
26
•31
I
•3585
7-24
75-71
S2
.09
I .2810
21
•58
82.66
23
.98
I
•3530
11.36
76.86
47
.08
1.3090
28
.18
80.42
22
•30
I
•3495
15-33
76.96
42
.66
i -3345
33
.80
79-25
20
• 40
I
•3485
I7.8l
77-14
39
.90
1-3465
37
.88*
77-37
19
.40*
I
•3485
I8.97*
77-15
38
•73*
I-3465
37
.64*
77-34
J9
.67*
I
•3485
19.34*
77-49
38.
,02*
) Results at 20° (N.).
Grams per ioo Grams H2O. Grams per ioo Grams H2O.
NaNO,
14.17
28-33
42.50
54-63*
35.91 NaCl
32.82 "
29.78 «
26.91 "
24.92* "
o NaCl
87.65 NaNO3
6-5
11
77-34
si
13.0
it
68.50
M
19-5
It
60.49
14
ioo gms. H2O dissolve 43.66* gms. NaNO3 + 26.58* gms. NaCl at 25°.
ioo gms. H2O dissolve 121.6* gms. NaNO3 + 17.62* gms. NaCl at 80°.
ioo gms. aq. alcohol of 40 wt. per cent dissolve 22.78 gms. NaNO3 + 10.17
NaCl at 25°.
* Indicates solutions saturated with both salts.
645
SODIUM CHLORIDE
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM NITRATE
AND VICE VERSA.
(Leather and Mukerji, 1913.)
Results at 30°.
, Gms. per 100 Gms.
atsol - -^2_ , S
Results at 40°.
Gms. per 100 Gms.
at Sol H?°- S
Results at 91°.
Gms. per 100 Gms.
£of H?0.
Solid Phase
in Each Case
>L NaN03. NaCl.
.202 0 36.3
.2j6 24.21 31.16
.343 48.15 26.35
.379 63.08 23.50
. 388 63 .40 23 . 40
.381 67.91 19.69
.394 81.46 9.76
. 406 95 . 90 o
"NaN03. NaCl.--
•197 o 36.53
.284 27.31 30.53
.323 54.82 26.50
.409 73.96 21.87
.397 74.01 21.71
.396 75.29 21. 61
.410 89.90 10.80
.421 105.2 o
NaN03. NaCl/
[.189 0 38.72
•296 37.43 30.21
.381 79.65 23.17
.487 127.2 17.05
.519 141.4 15.93
.518 141.3 15.83
.504 149.5 9-03
.521 160.8 o
NaCl
«
«
" f NaN03
" NaNO3
Results are also given at 20° which agree satisfactorily with those of Nicol.
Additional results at 30°, agreeing fairly well with the above, are given by Coppa-
doro (1913). Data for the solubility of sodium chloride in dilute solutions of
sodium nitrate at o° and at 25° are given by Armstrong and Eyre (1910-11).
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS 7.45 PER CENT SODIUM
SULFATE SOLUTIONS.
(Marie and Marquis, 1903.)
14.8
17.9
25.6
Gms. NaCl per
100 Gms. Sat. Sol.
23-30
23-33
23.485
27-75
32.18
34-28
Gms. NaCl per
100 Gms. Sat. Sol.
23.55
23.68
For additional data on this system see sodium sulfate, pp. 669 and 670.
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF ETHYL
ALCOHOL.
(Armstrong and Eyre, 1910-11.)
Results at o°.
Results at 25°.
Solvent Gms.
C2H5OH per
1000 Gms. H2O.
0
Gms. NaCl
per loo Gms.
Sat. Sol.
26.46
11.51
25-97
23-03
46.06
138.18
24.41
20.95
<*25 Of
Sat. Sol.
Solvent Gms.
C2H6OH per
1000 Gms. H2O.
Gms. NaCl
per 100 Gms.
Sat. Sol.
I .202
O
26.55
.196
11.51
26.06
.190
23-03
25.63
.179
46.06
24-75
.159
92.12
23.29
.1115
230.3
19.35
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS ALCOHOL AT 28°.
(Fontein, 1910.)
Gms. per 100 Gms. Sat. Sol.
Gms. per 100 Gms. Sat. Sol.
QH6OH.
H20.
NaCl.
O
73-53
26.47
3-8
71.6
24.6
7-7
69.7
22.6
16.1
64.6
19-3
25-3
58-9
15-8
35
52-5
12-5
C2HBOH.
H20.
NaCl.
45-35
45-35
9-3
56.2
37-5
6.3
67.4
28.9
3.7
78.8
19.7
1.5
89.6
10
0.4
Results are also given by Fontein showing the solubility of sodium chloride in
mixtures of ethyl alcohol, amyl alcohol and water at 28°, both when one liquid
phase is present and when conjugated liquid layers are formed.
SODIUM CHLORIDE 646
SOLUBILITY OP SODIUM CHLORIDE IN ALCOHOLS.
(At 18.5°, de Bruyn — Z. physik. Ch. 10, 782, '92; Rohland — Z. anorg. Ch. i89 327, '98.)
Gms. NaCl Gms. NaCl
t°. Alcohol. per too t°. Alcohol per 100
Gms . Alcohol . Gms . Alcohol ,
18.5 Abs. Methyl 1.41 room temp. Methyl ^15= 0.799 I-33
" Ethyl 0.065 Ethyl <Z15 =0.81 0.176
" Propyl<£15 =0.816 0.033
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS ETHYL ALCOHOL
SOLUTIONS.
(Bodlander — Z. physik. Ch. 7, 317, '91; Taylor — J. Phys. Ch. i, 723, '97; also Bathrick — Ibid, i,
159, '96.)
Results at 11.5° (B.). Results at 13° (B.).
Sp. Gr. of
Gms. per loo^cc. Solution.
Sp. Gr. of
Gms. per TOO cc. Solution.
Solutions. CgHeOH.
H2O.
Na
,C1.
Solutions.
C2H5OH.
H20.
NaCl.
I
•2035
O
86.62
31
•73
I
.2030
O
88.70
31.60
I
.1865
2
.86
86.14
29
.66
I
.1348
II. 8l
78.41
23.26
I
.1710
5
.41
83 -93
27
•77
I
.1144
J5-99
74.64
20. 8l
I
•1548
7
•93
81.50
26
•05
I
.0970
19-39
71-45
18.86
I
•1350
10
.84
78.78
24
.28
I
.0698
24-95
65.80
16.23
I
.1390
ii
.22
78.62
23
-65
I
.0295
32-33
57.96
12.66
I
.1088
16
•85
73-40
20
•63
O
.9880
40.33
49-34
9.13
O
•9445
49.28
38.54
5-93
0
•9075
57-91
29-37
3-47
o
.8700
63.86
21 .62
1.52
o
.8400
72 .26
11.24
0.50
Results at 30° and at 40° (T.).
Wt. per cent At 30°, Gms. NaCl per 100 Gms. At 40°, Gms. NaCl per TOO Gms.
Alcohol in Solvent. ' Solution. Water. Solution. Water.
o 26.50 36-05 26.68 36-38
5 24.59 34.29 24.79 34-69
10 32.66 32-57 22.90 33 .00
20 I9-o5 29.40 19.46 30.20
30 15.67 26.53 16.02 27.25
40 12.45 23.70 12.75 24.37
50 9 34 20.60 9.67 21.42
60 6.36 16.96 6.65 17.82
70 3.36 12.75 3-87 13 -^
80 1.56 7.95 1.69 8.68
90 0.43 4-30 0-50 5.10
100 gms. alcohol of 0.9282 Sp. Gr. = 45.0% by wt. dissolve at:
4° 10° 13° 23° 32° 33° 44° 5i° 6°°
10.9 ii. i 11.43 Il-9 I2-3 I2-5 I3-1 J3-8 14- 1 gms. NaCl
(Gerardin — Ann. chim. phys. [4] 5, 146, '56.)
ioo gms. of a mixture of equal parts of 96% alcohol and 98% ether
dissolve o.n gm. NaCl.
(Mayer — Liebig's Ann. 98, 205, '56.)
647 SODIUM CHLORIDE
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS METHYL ALCOHOL.
(Armstrong and Eyre, 1910-11.)
Results at o°. Results at 25°.
Solvent, Gms. Gms. NaCl Solvent, Gnu. Gms. NaCl
CH,OH per per 100 Gms. CH,OH per per 100 Gms.
1000 Gms. HaO. Sat. Sol. 1000 Gms. H20. Sat. Sol.
o 26.35 8.01 26.29
8.01 26.05 16.02 26.02
16.02 25.79 32.04 25.50
32.04 29.19 96.12 23.50
A sat. solution of NaCl in CH3OH contains o.i gm. NaCl per 100 gms. solution
at the critical temperature. (Centnerszwer, 1910.)
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS PROPYL ALCOHOL.
(Armstrong and Eyre, 1910-11.)
Aqueous propyl alcohol containing 15.01 gms. C3H7OH per 1000 cc. H2O dis-
solves 25.71 gms. NaCl per 100 gms. sat. solution at o° and 25.95 gms. at 25°.
Aqueous propyl alcohol containing 30.02 gms. C3H7OH per 1000 cc. H2O dis-
solves 25.12 gms. NaCl per 100 gms. sat. solution at o° and 25.37 gms. at 25°.
EQUILIBRIUM IN THE SYSTEM SODIUM CHLORIDE, NORMAL PROPYL ALCOHOL
AND WATER AT 23-25°.
(Frankforter and Frary, 1913.)
The authors determined the binodal curve and quadruple points of the system
but did not locate tie lines.
Gms. per 100 Gms. Homogeneous Liquid. Gms. per 100 Gms. {Homogeneous Liquid.
NaCl. C3H7OH. H2O.A NaCl. C3H7OH. H2O.'
0.55 87.7 11-75* 14-38 5-39 80.23
2.23 51.57 46.20 15.42 5.11 79.47
3-55 18.99 77-46 16.38 4.47 79.14
3.90 14.78 81.32 18.08 3.83 78.09
5.27 12.77 81.96 20. 12 3.27 76.61
8.04 9.49 82.47 22.35 2.64 7S-01
10.49 7-79 81.72 24.50 2.13 73.37
12.20 6.57 8l.23 24.9 2.3 72.8*
* Quad. pt.
The effect of temperature upon the equilibrium in the above system was greater
than observed in any of the other systems investigated and additional data, illus-
trating the extent of the temperature influence, are given.
100 gms. sat. sol. of NaCl in 99.6 per cent C3H7OH contain 0.04 gm. NaCl
at 25°. (Frankforter and Frary, 1913.)
EQUILIBRIUM IN THE SYSTEMS SODIUM CHLORIDE, ALLYL ALCOHOL, WATER, AT
20° AND SODIUM CARBONATE, ALLYL ALCOHOL, WATER, AT 20°.
(Frankforter and Temple, 1915.)
Results for Results for
NaCl + CH2 : CHCH2OH + H2O. Na2CO3 + CH2 : CH.CH2OH + H2O.
Gms. per 100 Gms. Alcohol + Water. Gms. per 100 Gms. Alcohol + Water.
rNaCl. Alcohol. Water. Na^CO,. Alcohol. Water.
3.509 69.867 30.133 0.456 61.112 38.888
4.452 64.858 33-142 0.708 56.334 43-666
5.079 60.821 39-179 i. on 51.930 48-070
6.712 54-683 45-3*7 1.468 48.109 5I-89i
8.776 47-132 52.868 2.580 41-052 58.948
10.650 40.392 59.608 3.414 37-I26 62.874
12.535 33-224 66.776 4.739 ,32.166 67.834
14.925 27.261 72.739 7-774 '23-753 76.247
18.557 I9-705 80.295 10.079 18.407 81.593
SODIUM CHLORIDE
648
SOLUBILITY OF SODIUM CHLORIDE IN. SEVERAL ALCOHOLS AT 25°.
(Turner and Bissett, 1913.)
Cms. Nad per
100 Cms. Alcohol.
1.31
o . 065
A, , ,
AlcohoL
Methyl Alcohol, CH3OH
Ethyl Alcohol,
C2H5OH
Propyl Alcohol,
Amyl Alcohol,
C3H7OH
C5HnOH
0.012
0.002
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS ACETONE SOLUTIONS AT 20°
(Frankforter and Cohen, 1914.)
Cms. per 100 Cms. Sat. Sol. Cms. per 100 Cms. Sat. Sol.
NaCl.
H20.
(CH3)2CO.
25-9
73-06
I.O4
24.19
71.18
4-03
20.85
66.78
12.37
18.32
63.16
18.52
17.89
62.21
19.90
NaCl.
H20.
(CH3)2CO.
16.55
61.59
21.86*
0-45
13-75
85.8*
0.32
13.92
85.76
o. 19
10.82
88.99
O.I2
8.94
90.94
* Quad pt.
Between the concentration 21.86 and 85.8 per cent acetone, two layers are
formed. The binodal curve corresponding to this range of concentration was
determined and it is stated by the authors that tie lines were located but the
analytical data for them are not given. The results for the binodal curve are as
follows:
Cms. per 100 Cms. Homogeneous Liquid.
Gms. per 100 Cms. Homogeneous Liquid.
NaCl.
H20.
(CH3)2CO.
0-59
15.46
83.95
0.79
17-58
81.63
0-93
18.83
80.24
1.27
22.19
76.54
i-57
23.89
74-54
2.31
27.27
70.42
4.87
36.79
58-34
'NaCl.
H20.
(CH3)2CO.
5-87
40.19
53-94
6-45
42. 12
51-43
7-53
46. 12
46.35
8.87
49-39
41.74
9-47
50.92
39.61
to. 35
53-o6
36.59
15-87
59-71
24.42
Additional data, showiner the effect of temperature on the above system, are
also given
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF:
Acetone at 20°.
(Herz and Knoch, 1904.)
cc. Acetone NaCl per.ioo cc.
per 100 cc. Solution.
Solvent. Millimols.
o 537-9
10 464.6
20 394.8
30 330.1
32 ) Lower layer 308 . 5
87 j Upper layer 7 . 7
88 7.3
90 4-3
Gms.
31-47
27.18
23.10
19.32
18.05
0-45
0-43
0.25
Glycerol at 25°.
(Herz and Knoch, 1905.)
Wt. Per cent NaCl per 100 cc.
Glycerol in Solution. Sp. Gr. of
Solvent.
Millimols.
Gms.
O
545-6
31-93
. 1960
13.28
501.1
29.31
.2048
25.98
448.4
26.23
•2133
45-36
370.2
21.66
.2283
54-23
333-9
19-54
• 2381
83.84
220.8
12.91
.2666
100*
167.1
9-78
.2964
* Sp. Gr. of Glycerol, 1.2592. Impurities about 1.5%.
100 gms. sat. solution in glycol contain 31.7 gms. NaCl at 14.8°.
(de Coninck, 1905.)
100 gms. H2O dissolve 236.3 gms. sugar -f- 42.3 gms. NaCl at 31.25°, or 100
gms. sat. aq. solution contain 62.17 gms. sugar + 11.13 gms. NaCl. (Kahler, 1897.)
649 SODIUM CHLORIDE
EQUILIBRIUM IN THE SYSTEM SODIUM CHLORIDE, METHYL ETHYL KETONE
AND WATER AT 25° (BINODAL CURVE).
(Frankforter and Cohen, 1916.)
Cms. per 100 Cms. Homogeneous Liquid. Cms. per 100 Cms. Homogeneous Liquid.
'NaCl. CH3.CO.QH6. H20. NaCl. CH3.CO.C2H5. HA
0.35 20.13 79.52 6.75 10.80 82.45
0-55 19-75 79-70 10.07 7-65 82.28
1.42 16.52 82.06 I4-32 5-36 80.32
1. 80 17.70 80.50 14.65 3.83 81.52
2.47 16.24 81.29 23-i5 2.08 74-77
4.11 13.34 82.55 24.14 0.94 74.92
SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF CARBAMIDE
(UREA) AND OF FORMAMIDE AT 25°.
(Ritzel, 1911.)
In Aqueous Carbamide. In Aqueous Formamide.
Cms. CO(NH2)2 Cms. NaCl Cms. HCO.NH2 Cms. NaCl
per 100 cc. per 100 cc. per 100 cc. per 100 cc.
Solution. Solution. Solution. Solution.
o 31-80 o 31-80
5 30-63 2.3 30.98
9-6 29.05 5.3 30.86
13 28.46 8 30.40
18 27.65 ii 29.11
23 27.24 15 28.52
28 26.56 18.8 27.76
According to results by Fastert (1912), the solubility of sodium chloride in
aqueous solutions of urea increases slightly with increase of urea in solution, thus:
Cms. CO(NH2)2 per 100 cc. Sol. 10 20 30 40 50
Cms. NaCl per 100 cc. Sol. 31.92 32.17 32.51 32.93 33.40
Data for equilibrium in the system sodium chloride, succinic acid nitrile, water
are given by Timmermans (1907).
loo gms. 95% formic acid dissolve 5.8 gms. NaCl at 19.7°. (Aschan, 1913.)
IOO gms. hydroxylamine dissolve 14.7 gms. NaCl at 17.5°. (deBruyn, 1892.)
100 cc. anhydrous hydrazine dissolve 8 gms. NaCl at room temp.
(Welsh and Broderson, 1915-)
FUSION-POINT DATA (Solubilities, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES.
NaCl + HC!. (Dernby, 1918.)
+ Na2CrC>4. (Sackur, 1911-12.)
+ NaCN. (Truthe, 1912.)
-j- NaF. (Ruff and Plato, 1903; Wolters, 1910; Plato, 1907.)
+ NaOH. (Scarpa, 1915.)
-j- Nal. (Ruff and Plato, 1903; Amadori, 19123.)
-j- NaNC>2. (Meneghini, 1912.)
+ Na4P2O7. (LeChatelier, 1894.)
-{- Na2SO4. (Ruff and Plato, 1903; janecke, 1908; Wolters, 1910; Sackur, 1911-12.)
-j- SrCU. (Vortisch, 1914; Sackur, 1911-12.)
-j- SrCO3. (Sackur, 1911-12.)
-j- T1C1. (Sandonnini, 1911, 1914.)
SODIUM CHROMATES 650
SODIUM CHROMATES (Mono, Di, etc.)
SOLUBILITY IN WATER.
(Mylius and Funk, 1900; see also Salkowski, 1901.)
Sodium Monochromate. Sodium Bichromate.
Gms. Na2 Mols. Na2 Gms. Na2 Mols. Na2
«. o CrO4 per CrO4 per Solid t o Cr2O7 per Cr2O7 per Solid
" * TOO Gms. 100 Mols Phase. 100 Gms. 100 Mols. Phase.
Solution.
H20.
Solution.
H2O.
0
24
.07
3
a^rC^.ioH^ O
6z.
98
II
.2
Na2Cr2O7.2H2O
10
33
.41
5
•55
17
63-
82
12
.1
41
18*
40
.10
7
•43
i8|
63-
92
12
.l6
"
18.
5
41
•65
7
•94
34-5
67.36
14
.2
"
19.
5
44
.78
9
.01
" 52
71 .
76
17
•4
M
21
47
.40
10
.00
72
76.
9
22
.8
M
25.
6
46
.08
9
a2CrO4.4H2O 8 1
79-
8
27
.1
"
31-
5
47
•05
9
.90
93
81.
19
29
.6
Na2Cr207
36
47
.98
10
• 2
98
8z.
25
29
.8
"
40
48
•97
10
.6
M
Sodium Tri Chromate.
A £
^\O
.20
II
••
T"0
V
Gms. I
sTa2
Mols.
Na2
49 •
5
50
•93
II
•5
to
Cr30,0
per
Cr3Ojo per
Solid
54-
5
52
.28
12
.2
•
11
100 Gms.
Solution.
100 Mols.
H20
Phase.
59-
5
53
•39
12
•7
o
80.
03
19
•9
Na2Cr3010.H20.
65
55
•23
13
•7
Na2Cr04 15^
80.44
2O
•4
"
70
55
•15
13
.6
IS
80.60
2O
•56
«•
80
55
•53
13
.8
55
82.68
23
•7
«
100
55
•74
14
.0
99
85.78
29
•9
"
* Sp. Gr. of sat. sol. at 18° = 1.432. f Sp. Gr. of sat. sol. at 18°
t Sp. Gr. of sat. solution at 18° = 1.745.
2.059
Sodium Tetrachromate.
Tetrasodium. Chromate.
Gms.
Mols.
Gms.
Mols.
1° ~
Na2Cr4Ol3
Na2Cr4Ol3
Solid
t°.
Na4Cr05
Na4CrO8
per zoo Gms.
Solution.
per 100
Mols.H2O.
Phase.
per 100 Gms. per 100
Solution. Mols.H2O.
O
72.96
10.5
Na2Cr4O,3.4H2O
O
33-87
4.II
16
74.19
II .2
it
10
35-58
4.42
18*
74.60
II .27
"
i8t
37-50
4.81
22
76.01
12-3
"
27.
7 40-09
5-38
37
45-13
6.62
Solid
Phase.
* Sp. Gr. of sat. solution at i8°=« 1.926.
t Sp. Gr. of sat. solution at 18° = 1.446.
A new hydrate of sodium chromate, Na2CrO4.6H2O, was found by Salkowski,
(1901) and the following data for its range of existence were determined.
f.
17.7
19.2
19.525
21.2
24.7
Gms.
NajCrO4
per 100
Gms.
Solution.
43.65
44.12
44-2*
44.64
45-75
Mols.
per 100 Solid Phase.
Mols.
H20.
8 . 62 Na2CrO4.ioH2O
8.77 "
... " +Na2CrO4.6H2O
8.96 Na2CrO4.6H2O
9-37
Gms.
Na2CrO4
per
100 Gms.
Sol.
25.9 46.3^
28.9
29.7
31.2
46.47
46.54
47.08
Mols.
Na,CrO«
per Solid Phase.
100 Mols.
H20.
9.57 Na2CrO4.6H2O
+Na2CrO4.4HzO
9.64
9.67
9.88
* This determination by Richards and Kelley (1911).
651
SODIUM CHROMATES
SOLUBILITY OF SODIUM CHROMATES IN WATER AT 30°.
(Schreinemakers, 1906.)
•
Composition in weight per cent:
Of Solution. Of Residue.
%Cr03.
%Na20.
o
±42
2.00
41.44
2.04
40.89
4-23
35 -51
6.64
32-34
15.19
27.06
10-22
29-39
8-93
28.49
8.62
26.91
13 .12
23.91
18.44
22.86
19.26
22.98
17.84
24.21
28.82
17.88
38.93
16.30
48.70
16.49
50.68
15-72
58.08
13-89
66.13
13.70
65.98
14-15
68.46
10.95
66.88
9-85
70.06
11.85
69.04
11.04
67.84
9.81
64.48
4-51
62.28
0-0
%Cr08.
27.52
27.72
37-07
I5-48
18.09
%Na20.
5.83 42.64
36.57
34-60
32.20
28.41
26.89
18.57 25.92
21.54
25-31
26.24
24-98
31-97
23-47
40.70
20.83
47-49
19-75
62.76
I7-38
69.48
16.06
69.46
15.15
73.88
I3-38
71.27
10.67
83 -95
9-57
81.80
6-43
82.85
5-42
79-49
2.71
Solid Phase.
NaOH.H2O
NaOH.H20 + Na2Cr04
Na2Cr04
Na2Cr04.4H20
Na2CrO4.
Na2Cr30,0.H20
Na2Cr3Oio.H20 + Na2Cr4Ql3^HaO
Na2Cr30l3.4HaO
Cr08
100 gms. of a saturated aqueous solution contain at 30°:
46.627 gms. Na2CrO4, or 100 gms. H2O dissolve 87.36 gms. Na2CrO4.
66.4 gms. Na2Cr2O7, or 100 gms. H2O dissolve 197.6 gms. Na2Cr2O7.
100 gms. absolute methyl alcohol dissolve 0.345 Sms. Na2CrO4 at 25°.
(de Bruyn, 1892.)
Data for equilibrium in the system sodium chromate, sodium sulfate and water
at 15° and at 25° are given by Takenchi (1915). The mixtures were rotated at
constant temperature until attainment of equilibrium and both the saturated
solutions and the undissolved residues were analyzed. Very extensive tables of
results are given. The decahydrates of sodium and chromium are isomorphous
and the results show that these two salts are mutually miscible in all proportions
at 15°. At 25° the solubility curve consists of three branches. The solutions of
the first branch are in equilibrium with decahydrated mixed crystals, those of the
second branch with anhydrous sulfate and those of the third with both anhydrous
sodium sulfate and hexahydrated sodium chromate.
SODIUM CHROMATES 652
SOLUBILITY OF SODIUM DICHROMATE IN ALCOHOL AT 19.4°.
(Reinitzer, 1913.)
An excess of Na2Cr2O7.2H2O was shaken with absolute alcohol for 10 minutes
and the mixture filtered. The filtrate contained 5.132 gms. NaaC^Oy^I^O per
100 cc. and its d\$.i was 0.8374. The solution decomposed within a few minutes
with production of a brown precipitate and evolution of an aldehyde odor. The
results are, therefore, only approximately correct.
SODIUM CINNAMATE C6H5CH:CHCOONa.
100 gms. H2O dissolve 9.1 gms. sodium cinnamate at 15.20°.
100 cc. 90% alcohol dissolve 0.625 Sm- at 15-20°. (Squire and Caines, 1905.)
SODIUM CITRATE (CH2)2COH(COONa)8.5iH2O.
SOLUBILITY IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Wt. Per cent •, nf Gms. C6H5O7Na3.- Wt. Per cent
QH5OH in c * c i S5H2O per 100 Gms. QHsOH in
Solvent. Sat. Sol. Solvent.
d2Bo{ Gms.C6H5C
0
1.276
48.1
40
o-953
4-5
10
I .190
37-4
50
0.918
1-4
20
1. 100
25
60
0.892
0.3
30
1. 006
ii. 8
100
0.789
0
Data for equilibrium in the system sodium hydroxide, citric acid, phosphoric
acid and water at 20° are given by Pratolongo (1913).
The author fails to describe clearly the terms in which the results are expressed,
consequently their exact meaning is not clear.
SODIUM (Ferro) CYANIDE Na4Fe(CN)6.
SOLUBILITY IN WATER.
(Conroy, 1898.)
t°. 20°. 42°. 80°. 98-5°.
Gms. Na4Fe(CN)e per 100 gms. H^O 17.9 30 . 2 59 . 2 63
SODIUM FLUORIDE NaF.
100 gms. sat. aq. solution contain 4.3 gms. NaF at 18°. Sp. Gr. of solution =
1.044. (Mylius and Funk, 1897.)
SOLUBILITY OF SODIUM FLUORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
FLUORIC ACID AT 21°.
(Ditte, 1896.)
Gms. per 1000 Gms. H2O. Gms. per 1000 Gms. H20.
o HF
4i
.7 NaF
83.8
HF
22.9 NaF
10
(i
4i
-4
1C
129.7
tt
23.8
((
45-8
tt
22
•5
(I
596.4
tt
48.8
((
56.5
a
22
-7
ft
777-4
it
81.7
It
FUSION-POINT DATA (Solubility, see footnote, p. i) ARE GIVEN FOR THE
FOLLOWING MIXTURES.
NaF + FeF3. (Puschin and Baskov, 1913-)
" +ZnF3.
+ Nal. (Ruff and Plato, 1903.)
+ NaOH. (Scarpa, 1915.)
+ Na2SO4. (Wolters, 1910.)
SODIUM FLUOSILICATE Na2SiF6.
100 gms. H2O dissolve 0.65 gm. at 17.5°, and 2.45 gms. at 100°. (Stolba, 1872.)
653
SODIUM FORMATE
SODIUM FORMATE HCOONa.
SOLUBILITY IN WATER.
(Groschuff, 1903.)
— 20
O
+ 15
18
18
21
23
Gms. Mols.
HCOONa HCOONa
per ioo Gms per ioo Mols.
Solution.
22.80
30-47
41.88
44.92
44-73
46.86
48.22
H20.
7.82
ii. 6
19.1
21.6
21.4
23-3
24.65
Solid
Phase.
HCOONa.3H2O
HCOONa.2H2O
Gms.
HCOONa
Mols.
HCOONa
Solid
" per ioo Gms. per ioo Mols
Phase.
Solution.
H20.
25-
5 50-53
27.0
HCOONa.2H30
18
49.22
25-65
HCOONa
29
50-44
26.9
"
54
53-8o
30.8
M
74-
5 56-82
34-8
44
ioo.
5 6l-54
42-35
44
123
66.20
44
Sp. Gr. of the saturated solution of the dihydrate at 18° = 1.317.
SOLUBILITY OF SODIUM ACID FORMATE (EXPRESSED AS NEUTRAL
SALT) IN AQUEOUS SOLUTIONS OF FORMIC ACID.
(Groschuff.)
Gms. Mols.
to HCOONa HCOONa
' per ioo Gms. per ioo Mols-
Solution. H2O.
o 22.35 T9-5
25.5 29.62 28.45
66.5 41.08 47-1
Solid
Phase.
HCOONa.HCOOH
Gms. Mols.
to HCOONa HCOONa Solid
' per ioo Gms. per ioo Mols. Phase.
Solution. 'H2O.
45-5
70
85
38.8S
41.27
43-09
HCOONa
47-5
51-2
SODIUM GLYCEROPHOSPHATE (Disodium) OP(OC3H7O2)(ONa)2.5H2O.
ioo gms. sat. solution in H2O contain 27.38 gms. of the anhydrous salt at 18°.
(Rogier and Fiore, 1913.)
SODIUM HYDROXIDE NaOH.
SOLUBILITY IN WATER.
(Pickering, 1893; Mylius and Funk (Dietz)
Gms. NaOH
t°. per ioo Gms.
Solution
, Water.
- 7-8
8.0
8-7
— 20
16.0
19.1
-28
19.0
23-5
-24
22.2
28.5
-17.7
24-5
.32-5
0
29.6
42 .0
+ 5
32.2
47-5
10
34-o
51 .5
15.5
38-9
63-53
5
45-5
83-5
12
50-7
103.0
Ice
Solid
Phase.
aOH.7H2O
NaOH.7H2O + NaOH-sH2O
NaOH.5H2O + NaOH4H2O a
NaOH.4H2O a
NaOH.4H2O a + NaOH3iH2O
NaOH.3iH2O
f. pt.
NaOH.s JHjsO -f NaOH-zH^
Dietz)
, 1900.)
Gms.
NaOH
^o. per ioo Gms.
Solid
Phase.
Solution,
. Water. "
20
52.2
IOO
NaOH-HaO
30
54-3
1 19
44
40
56.3
129
M
50
59-2
145
M
60
63-5
174
M
64.
369.0
222-3
" f . Pt.
6l.
874.2
288
NaOH.H2O
H-NaOH
80
75-8
3r3
NaOH (?)
no
78.5
365
"
192
83-9
52i
M
Sp. Gr. of sat. solution at 18° = 1.539.
For determinations of the Sp. Gr. of sodium hydroxide solution, see Kohlrausch,
1879; Wegscheider and Walter, 1905.
ioo gms. of the sat. solution in water contain 46.36 gms. NaOH at 15°.
(de Forcrand,
SODIUM HYDROXIDE
654
1000 gms. liquid ammonia dissolve 0.0025 Sm- NaOH at —40°.
(Skossareswky and Tchitchinadze, 1916.)
Data for equilibrium in the system sodium hydroxide, resorcinol and water at
30° are given by van Meurs (1916).
Fusion-point data for NaOH + Nal are given by Scarpa (1915).
SODIUM IODATE NaIO3.
SOLUBILITY IN WATER.
t°.
Gms. NalOs per 100 gms.
(Gay-Lussac; Kremers, i8s6a.)
o .
2-5
20°.
9
40 .
15
60°.
21
80°.
27
100 ,
34
EQUILIBRIUM IN THE SYSTEM SODIUM IODATE, IODIC ACID AND WATER AT 30°.
(Meerburg, 1905.)
ioo Gms. Sat. Sol
HIO,.
NaI03.
•» ouiiu .rnase.
O
9.36
NalOj.iiHjO
1.98
9-52
"
4-86
10.22
"
5.86
11.04
«
7.40
II. 60
" unstable
9-73
14.73
« «
6.70
II. 21
" +Na2O.2l2<
7.80
10.30
NaA2l»C
9.15
9
"
9-93
8.71
"
Gms. per TOO Gms. Sat. Sol.
Solid Phase.
HIO3.
NaI03.
11.20
7-54
Na2O.2lA
11.82
7.20
" +NaIO3.2HIO3
11.62
5.65
NaI03.2HIO,
23.23
3-69
"
32.68
2.91
"
46.62
2.67
"
55.48
2.12
«
65.47
1.83
"
76.19
1.42
+HIO,
76.7Q
0
HIO,
SODIUM IODIDE NaI.2H2O.
SOLUBILITY IN WATER.
(de Coppet, 1883; see also Etard, 1884; and Kremers, i8.<;6a.)
t°
Grams Nal
per ioo Gm;
5- Solid
Water.
Solution.
Phase.
— 2O
148.0
59-7
NaI.2H2O
O
I58-7
61 .4
it
10
168.6
62.8
*
20
178.7
64.1
M
25
184.2
64.8
H
30
190.3
65.6
"
40
205.0
67.2
"
50
227.8
."
t°.
Grams Nal
per ioo Gms.
Solid
Phase.
' Water.
Solution.
60
256.8
72.0
NaLaHaO
65
278.4
73-6
"
67
' 293
74.6
Nal
70
294
74-6
"
80
296
74-7
M
IOO
302
75.1
It
120
310
75-6
•
140
32I
76.3
«
The eutectic mixture of Ice + NaI.sH2O is at —31.5° and contains about 39
per cent Nal. (Meyerhoffer, 1904.)
The tr. pt. for NaI.sH2O + NaI.2H2O is at —13.5 and the saturated solution
contains 60.2 gms. Nal per 100 gms. (Panfiloff, iSgaa.)
The tr. pt. for NaI.2H2O + Nal is at 64.3° and the saturated solution contains
74.4 gms. Nal per 100 gms. (Panfiloff, 1893.)
100 gms. HaO dissolve 172.4 gms. Nal at 15° and the d\6 of the sol. is 1.8937.
(Greenish, 1900.)
100 gms. sat. solution in H2O contain 65.5 gms. Nal at 30°. (Cocheret, 1911.)
SOLUBILITY OF SODIUM IODIDE IN ALCOHOLS AT 25°.
(Turner and Bissett, 1913.)
loo gms. Methyl alcohol, CH3 OH dissolve 90.35 gms. Nal.
Ethyl " C2HBOH " 46.02
Propyl " C3H7OH " 28.22
Amyl " C6HUOH " 16.30
655
SODIUM IODIDE
SOLUBILITY OF SODIUM IODIDE IN AQUEOUS ETHYL ALCOHOL AT 30°.
(Cocheret, 1911.)
Nal.
C2H6OH.'
ounu jriioac.
65.52
O
NaI.2H2O
64
3-42
"
54-2
18.S
ii
48.8
28.5
«
42.35
41.7
"
Gms. per 100 Cms. Sat. Sol.
'~NaL CzH6OH".
38.5 53-2
37-49 55-37
35.65 59.24
33-24 61.78
30.90 68.70
Solid Phase.
NaI.2H20
" + Nal
Nal
Data are also given for the solubility of mixtures of Nal + Na2CO3 in aqueous
ethyl alcohol at 30°.
SOLUBILITY OF SODIUM IODIDE IN ABSOLUTE ETHYL ALCOHOL AT TEMP-
ERATURES UP TO THE CRITICAL POINT.
(Tyrer, igioa.)
IO
30
IOO
Gms. Nal per
loo Gms. C2H6OH
43-77
44-25
44-50
45
45-i
f o Gms. Nal per
loo Gms. QjHsOH.
1 2O
160
180
45-2
45
44-3
2OO
22O
230
42-3
38.5
36.2
240
250
255
260
261.5*
Gms. Nal per
loo Gms.
32-7
26.2
21
10.8
8.6
' crit. t. of solution.
The mixtures were placed in sealed glass tubes which were heated in a specially
constructed, electrically heated air bath. The temperature at which the last
trace of salt just dissolved was determined in each case. The experiments were
made with very great care. Results are also given for the solubility of sodium
iodide in the vapor of ethyl alcohol above the critical point.
SOLUBILITY OF SODIUM IODIDE IN MIXTURES OF ALCOHOLS AT 25°.
(Herz and Kuhn, 1908.)
In CHsOH + C2H6OH. In CH3OH + C3H7OH. In C2H6OH +
Per cent
d of
Gms. Nal
Per cent
A - of
Gms
Nal
Per cent
dapoi
Gms. Nal
CH3OH in
Mixture.
.3.5 Ui>
Sat. Sol.
per 100 cc.
Sat. Sol.
C3H7OHin (
Mixture. •
U2A Wi
sat. Sol.
peri
Sat.
30 CC.
Sol.
C3H7OHin (
Mixture.
>at. Sol.
per loo cc.
Sat. Sol.
0
.0806
35-15
O
•3250
63
22
O
.0806
35-15
4.37
.1029
37-68
II. II
-2853
58
45
8.1
.0732
34.60
10.4
.1123
38.71
23.8
.2528
54
64
17-85
.0720
34.05
41.02
.1742
45.98
65-2
.1387
40
71
56.6
.0276
28.41
80.69
.2741
57-44
91.8
.0420
29
14
88.6
.0130
26.13
84.77
.2886
58.92
93-75
.0178
26
49
91. 2
.0104
25.88
91.25
-3056
61.10
IOO «
>.9968
24
ii
95-2 i
[.OO2O
24.74
IOO
.3250
63.22
IOO <
>.9968
24.11
SOLUBILITY OF SODIUM IODIDE IN SEVERAL SOLVENTS.
(At 22.5°, de Bruyn, 1892; at ord. temp. Rohland, 1898; Walden, 1906.)
Solvent.
Gms. Nal
per loo Gms.
Solvent.
Solvent.
Gms. Nal per 100 cc.
Sat. Solution.
Absolute Ethyl Alcohol 22.5 43 . i
Ethyl Alcohol, d\5 = 0.810 ord. temp. 58. 8
Absolute Methyl Alcohol 22.5 77 . 7
Methyl Alcohol, d\$ = 0.799 ord. temp. 83 . 3
Propyl Alcohol, d^= 0.816 ord. temp. 26.3
at o°. at 25°.
Acetonitrile 2 2 . 09 1 8 . 43
Propionitrile 9.09 6.23
Nitro Methane 0.34 0.48
Acetone very soluble
Furfural ... 25.10
SODIUM IODIDE
656
SOLUBILITY OF SODIUM IODIDE IN ACETAMIDE.
. (Menschutkin, 1908.)
Gms. per 100 Gms.
Sat. Sol.
Solid Phase;
NaI.2CHr _ NaT
CONH2 - NaL
82 m.pt.ofpureacetamide CHsCONHj
78
9-5
5-32
74
18
10.08
70
25-5
14
66
3i-9
17.86
62
37-3
20.9
58
41.9
23-44
54
46.1
25-8
50
50
28
46
53-7
30.1
41-5
57-7
32-3
+NaI.2CH3CONH2
Gms. per 100 Gms.
t°. Sat. Sol.
Solid Phase.
NaI.2CHr
CONH2
= NaI.
50
59
33
NaI.2CH3CONH,
60
60.S
33-9
"
70
62.2
34-8
"
80
64.2
35-9
«
90
66.5
37-2
«
IOO
69.2
38.7
"
no
72.6
40.6
«
1 20
78.7
44
«
125
84.7
47-4
" +NaI
150
85.1
47-7
Nal
175
85.5
47-9
"
loo cc. anhydrous hydrazine dissolve 64 gms. Nal at room temp.
(Welsh and Broderson, 1915.)
SODIUM IODOMERCURATE
A saturated solution at 24.75°, prepared by adding Nal and HgI2 in excess to
water, contained 4.59% Na, 25% Hg, 58.25% I and 12.2% H2O, corresponding
to 0.20 mol. alkali, 0.12 mol. Hg and 0.45 mol. I. (Duboin, 1905.)
SODIUM MOLYBDATE Na2MoO4.
SOLUBILITY IN WATER.
(Funk, igooa.)
Gms.
Mols.
Gms.
t°.
Na2MoO4
per loo Gms.
Solution.
Na2MoO4
per loo
Mols. H2O.
Solid Phase. t°.
Na2MoO4
per loo Gm
Solution.
o
30-63
3-86
Na2MoO4.ioH2O 15-5
39.27
4
33.83
4-47
18
39-40
6
35.58
4-83
32
39.82
9
38.16
5-39
" 5z-5
41.27
10
39-28
5-65
Na2MoO4.2H2O IOO
45-57
Mols.
&»»»-"•
lols. H2O.
5.65
5.70
5.78
6.14
7-32
d of the sat. sol. at 18° is 1.437.
100 gms. H2O dissolve 3.878 gms. sodium trimolybdate, Na2Mo3Oi0, at 20°, and
13-7 gms. at 100°. lUffik, 1867.)
i oo cc.H2O dissolve 28.39 gms. Na2O.4MoO3.6H2Oat2i°,(fj5 = 1.47. (Wempe, 1912.)
Fusion-point data for Na2MoO4 + Na2WO4 and Na2MoO4 + NazSO4 are given
by Boeke (1907).
SODIUM NITRATE NaNO3.
SOLUBILITY IN WATER.
(Mulder; Berkeley, 1904; see also Ditte, 1875; Maumee, 1864; Etard, 1894.)
Gms.
NaNO3per looGms. Mols. per
t°
Gms. NaNOj per 100 Gms.
Mols. per
Solution.
Water.
Liter.
I .
Solution.
Water.
Liter.
O
42
.2
72.
9- 73 *
6.7I*
80
59-
7
148
-I48. *
10-35*
IO
44
•7
80.
8- 80.5
7.l6
IOO
64-
3
180
-175.8
II-30
20
46
•7
87.
5-88
7.60
1 2O
68.
6
218
-208. 8f
I2.22f
25
47
.6
91
- 92
7.8o
180
78.
I
356.
7
30
48
-7
94-
9- 96.2
8.06
220
83.
5
506
40
50
•5
IO2
-104.9
8.51
225
91.
5
1076
50
52
.8
112
-114
8-97
3!3t
IOO
oo
00
54
•9
122
-124
9.42
*
Berkeley.
T at 119°.
J m.pt.
657
SODIUM NITRATE
SOLUBILITY OF SODIUM NITRATE IN AQUEOUS AMMONIA SOLUTIONS AT 15°.
(Fedotieff and Koltunoff, 1914.)
In Aqueous NH3.
In Aqueous NH3 + NH4NO3.
duoi
Sat Sol.
I.2S3
1-233
I. 212
Cms. per 100 Gms. H2O.
NH3.
13.87
17.28
20.38
NaNO3.
75.03
73-99
73.18
d15of
Sat. Sol.
Gms
. per 100 Gms.
H20.
NH3.
NHUNO-,.
NaNO,.
1.324
1-330
12.91
16.97
83.51
128.9
74.10
69.40
SOLUBILITY OF SODIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT o°.
(Engel, 1887; see also Schultz, 1860.)
valents per 10 cc. Solution. SD. Gr. of
Grams per TOO cc. Solut
NaNO3.
HNO3.
NaNO3.
HNO3.
66.4
0
-341
56.5
O-OO
63-7
2-65
•338
54-2
1.67
60.5
5-7
•331
51.48
3-59
56-9
8.8
.324
48.42
5-55
52-75
12-57
.312
44.88
7.92
48.7
16.9
•308
41.44
10.65
39-5
27.0
.291
33 -61
17.02
35-1
32-25
.285
29.86
20.33
3i-i
37-25
.282
26.46
23.48
23-5
48.0
.276
20. o
30.26
18.0
57-25
.276
*5-32
36.09
12.9
71.0
.291
10.97
44.76
SOLUBILITY OF MIXTURES OF SODIUM NITRATE AND POTASSIUM NITRATE
IN WATER AT 20°.
(Carnelly and Thomson, 1888.)
Per cent
NaNO3 in
Mixtures
Gms. per 100 Gms.
H20.
Used.
NaN03.
KN03.
100
86.8
0
90
96.4
13.2
80
98.0
38.5
60
90.0
47-6
50
66.0
40.0
Per cent
NaNO3 in
Mixtures
Gms. per 100
H20.
Gms.
Used.
NaN03.
KNO3.
45-7
53-3
34.7
40
45 -6
35-5
20
20.8
33-3
10
9-4
31-5
O
o.o
33-6
100 gms. H2O dissolve 24.9 gms. NaCl + 53-6 gms. NaNO3 at 20°.
(Rudorff, 1873; Karsten; Nicol, 1891.)
-UBILITY
OF SODIUM
NITRATE IN AQUEOUS
SOLUTIONS OF SODIUM
HYDROXIDE AT o°.
(Engel, 1891.)
Milligram Mols. per 10
cc. Solution.
Sp. Gr.
of
Grams per 100 cc.
Solution.
Na20.
NaN03.
Solutions.
NaOH.
NaNO3.
O-O
66.4
I-34I
o.o
56-50
2.875
62-5
I-338
2.30
53-19
6.1
57-15
1-333
4.89
48.63
12-75
47-5
•327
IO.2I
40.42
26.0
29-5
-326
20.83
25.10
39-o
17-5
•332
3I-25
14-89
45-88
I3-I9
•356
36.76
II .22
60.88
6.05
.401
48-75
5-15
SODIUM NITRATE
658
Data for equilibrium in the system sodium nitrate, sodium sulfate and water at
10°, 20°, 25°, 30°, 34° and 35° are given by Massink (1916, 1917).
SOLUBILITY OF SODIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM
THIOSULFATE.
(Kremann and Rodemund, 1914.)
Results at 9°.
Cms. per 100 Gms.
Sat. Sol.
NaNO3.
33-31
22.57
4.22
Na2S203.
12.26
23-4I
34-77
Solid Phase.
NaN03
" +Na2S203.SH20
NaaSA.53
Results at 25°.
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
NaNO3.
Na2S2O3.
35-42
12.72
NaN03
25.40
19.90
18.02
24.25
3I.8I
32.83
" +Na2S203.SHzO
Na2S203.sH20
4-33
40.50
"
SOLUBILITY OF SODIUM NITRATE IN ALCOHOLS.
100 gins. abs. methyl alcohol dissolve 0.41 gm. NaNO3 at 25°.
100 gms. abs. ethyl alcohol dissolve 0.036 gm. NaNO3 at 25°.
(de Bruyn, 1892.)
SOLUBILITY OF SODIUM NITRATE IN AQUEOUS ETHYL ALCOHOL AT
DIFFERENT TEMPERATURES.
(Bodlander, 1891; Taylor, 1897; Bathrick, 1896.)
Results at 13° (B.).
Sn Or of Gms. per 100 cc. Solution.
Results at 16.5° (B.).
So.Gr.of Gms. per 100 cc. Solution.
Solutions.
QsH6OH.
H20.
NaNO3.
Solutions.
C6H5OH.
H2O.
NaNO3.
1.3700
O-O
75
•34
6l
.66
I
3745
o.o
75
•25
62 -2O
*-3395
3-08
73
•53
57
•34
j
,3162
6.16
70
.82
54-64
1.3120
6.01
7i
.81
53
•39
j
.2576
II .60
68
.10
46.06
1.2845
8.30
70
•85
49
•3o
I
.2140
16.49
65
.04
39-87
1.2580
10.91
69
•47
45
.42
j
.1615
22.17
61
-67
32-3I
1-2325
13-77
67
.12
42
•36
j
•0855
32.22
S2
.92
23-4I
I.2OIO
16.46
66
.16
37
.48
I
•0558
37-23
48
•50
19.85
I
.0050
43-98
42
.78
13-74
0
.9420
52.60
32
•13
9-47
0
.9030
6o.OO
25
•65
4-65
0
.8610
63.16
21
•31
1.63
Results at 30° (T.).
Wt. per cent
Alcohol in
Gms. NaNO3
per 100 Gms.
Solvent.
Solution.
Water-
0
49-10
96.45
5
46.41
9I-I5
10
43-50
85-55
20
37-42
74-75
30
3i-3i
65.10
40
25.14
55-95
50
18.94
46.75
60
12.97
37-25
70
7.81
28.25
90
1. 21
12.25
Results at 40° (Bathrick).
Gms. NaNOs
per 100 Gms.
Aq. Alcohol.
Wt.
"per cent
AlcohoL
O
8.22
17.4
26.O
36.0
42.8
55-3
65-1
77-o
87.2
104-5
90.8
73-3
61
48
40.6
27
18
9-4
4.2
659
SODIUM NITRATE
SOLUBILITY OF SODIUM NITRATE IN AQUEOUS ALCOHOL AT 25°.
(Armstrong and Eyre, 1910-11.)
Solvent.
Mols. C2H5OH
per 1000 Gms. HjO.
O
0.25
0.50
I
2
Gms. C2H6OH
per 1000 Gms. H2O.
O
23.03
46.06
Q2.I2
Gms. NaNO,
per loo Gms.
Sat. Sol.
47-93
47.32
46.73
45-43
43-04
SOLUBILITY OF SODIUM NITRATE IN AQUEOUS SOLUTIONS OF ACETONE.
Results at 30°.
(Taylor, 1897.)
Wt. per cent
Acetone in
Solvent.
0
5
Gms. NaNO3
per ioo Gms»
Solution.
49-10
46.96
Water.
96.45
93.20
9.09
20
45-11
40.10
90.40
83.70
3°
40
60
29.80
24-34
77-20
70-75
64.40
59-95
70
80
00
7.10
I.Q8
50-50
38.20
20.20
Results at 40°.
(Bathrick,
1896.)
Wt. Gms. NaNOs
per cent p
er ioo Gms.
Acetone. A
LQ. Acetone.
o.o
105
8.47
91.2
16.8
78-3
25.2
66.4
34-3
57-9
44.1
46.2
53-9
32-8
64.8
23.0
76.0
10.8
87.6
3-2
IOO gms. hydroxylamine dissolve 13.1 gms. NaNO3 at 17-18°. (de Bruyn, 1892.)
100 cc. anhydrous hydrazine dissolve 100 gms. NaNO3 at room temp.
(Welsh and Broderson, 1915.)
Fusion-point data for NaNO3 + NaNOa are given by Bruni and Meneghini
(1909, 1910).
Results for NaNO3 + SrNO3 + KNO3 are given by Harkins and Clark (1915)
and results for NaNO3 + T1NO3 by van Eyk (1905).
SODIUM NITRITE
NaN02.
SOLUBILITY IN WATER.
(Oswald, 1912, 1914.)
Gms. NaNO2
loo Gms. Sat.
4-5
9
12
-12.5
9.1
23.8
29.6
i5.5Eutec. 39.7
8 40.8
o 41-9
43-8
Solid Phase.
Ice
+NaNO,
NaNOj
10
20
45.8 (d= 1.3585) "
30
40
52
65
81
92
103
128
Gms. NaNO2 per c ,• , p« aci
loo Gms. Sat! Sol. Solld Phase'
47-8
49-6
51.4
54.6
57.9
59-7
62.6
68.7
NaNOj
(Divers, 1899.)
ioo gms. H2O dissolve 83.3 gms. NaNO2 at 15°.
100 gms. H2O dissolve 83.25 gms. NaNO2 at 15°.
(v. Niementowski and v. Roszkowski, 1897.)
ioo gms. H2O dissolve 73.5 gms. NaNO2 at 15°, di6 = 1.3476.
(Greenish and Smith, 1901.)
SODIUM NITRITE 660
SOLUBILITY OF SODIUM NITRITE IN AQUEOUS SOLUTIONS OF SODIUM
NITRATE AND VICE VERSA AT SEVERAL TEMPERATURES.
(Oswald, 1912, 1914.)
Results at o°.
Results at 21°.
Results at 52°.
Results at 103°.
jms. per 100 Gms. H2O.
Gms. per 100 Gms. H2O.
Gms. per 100 Gms. H2O.
Gms. per 100 Gms. H2O.
'NaN02.
NaN03. '
' NaNO2.
NaNOj.
NaNO2.
NaNOj.
NaNO2.
NaNOa. '
73
0
84.75
0
108.8
0
166
O
68
19
81.1
9.6
104.3
20.6
153-3
33-2
67
36.3
79-7
23-5
99-5
43-2
148.8
58.8
64.9
41.7*
73-8
50.8
98.8
82 *
142.4
116 *
50-3
46.8
54.5*
65.2
88
100
126.8
30.2
55-4
64.2
56.7
44.2
92.9
60. i
142.9
0
74.2
46.8
62.8
27.2
101.4
0
181.2
21.6
74-7
14.7
109
o
89.3
0
118
* Both salts in solid phase.
Similar results are also given for 18°, 65°, 81° and 92°.
100 gms. H2O, simultaneously saturated with both salts, contain 53.9 gms.
NaNO2 + 1 1. 8 gms. Na2SO4 at 16°. (Oswald, 1914.)
SOLUBILITY OF MIXTURES OF SODIUM NITRITE AND SILVER NITRITE IN WATER
AT 14° AND AT 22°. (See also p. 620.)
(Oswald, 1912, 1914.)
Results at 14°. Results at 22°.
Gms. per 100 Gms. H2O. Gms. per 100 Gms. H2O.
tfaNOT AiNO;. tfaNOT AiN02. SoMPhaaem Each Case.
55 15.2 58.3 21.5 AgN02+Na2Ag2(N02)4.H20
74-7 II- 3 78.3 13.4 NaNQ,+NagAg8(NOj)4.H,0
100 gms. abs. methyl alcohol dissolve 4.43 gms. NaNO2 at 19.5°.
100 gms. abs. ethyl alcohol dissolve 0.31 gm. NaNO2 at 19.5°. (de Bruyn, 1892.)
SODIUM RHODONITRITE Na6Rh2(NO2)i2.
100 gms. H2O dissolve 40 gms. at 17°, and 100 gms. at 100°. (Leidie, 1890.)
SODIUM OLEATE C8Hi7CH:CH(CH2)7COONa.
SOLUBILITY IN WATER AND AQUEOUS BILE SALTS.
(Moore, Wilson and Hutchinson, 1909.)
c i i. Gms. Oleate per
Solvent- 100 Gms. Sat. Sol.
Water 5
Aq. 5% Bile Salts 7.6
Aq. 5% Bile Salts + i% Lecithin n .6
SODIUM OXALATE Na2C2O4.
SOLUBILITY IN WATER.
(Souchay and Leussen, 1856; Pohl, 1852.)
t°. 15.5°. 21.8°. f 100°.
Gms. Na2C2O4 per 100 gms. H2O 3.22 3 . 74 6 .33
100 gms. sat. solution of sodium oxalate in water contain 3.09 gms. NajC2O4 at
15° and 4.28 gms. at 50°. (Colani, 1916.)
loo gms. 95% formic acid dissolve 8.8 gms. Na2C2C>4 at 19.3°. (Aschan, 1913.)
66i
SODIUM OXALATE
SODIUM OXALATE
SOLUBILITY OF MIXTURES OF SODIUM OXALATE AND OXALIC ACID IN
WATER AT 25°. (Foote and Andrew, 1905.)
Solid
Phase.
Gms. per 100 Cms.
Solution.
Mols. per 100 Mols.
H2O.
H2C204. Na2C204".
H2C204.
Na2C204.
10.20
2.274
10.50 0.83
2.370
0.130
9.15 0.71
2.032
0.106
6.88 0.86
1-493
0.125
1.14 1.25
0.234
0.172
0.47 3.20
0.098
o . 446
0.42 3.85
0.090
0.541
3.60
0.502
HaC204.2H20 + HNaC204.H20
Double Salt, HNaC2O4.H2O
HNaC2O4.H2O + Na^^
Na2C204
SOLUBILITY OF MIXTURES OF SODIUM OXALATE AND OTHER SODIUM SALTS
IN WATER AT 15° AND AT 50°. (Colani, 1916.)
Gms. per 100 Gms. Sat. Solution.
i5
0.
027
Na2C204
+
26.28
NaCl
o.
063
H
+
26.64
H
i5
0.
86
"
+
IO.26
Na2S04
0.
22
((
+
31-95
tt
15
0.
051
"
+
45.86
NaN03
5o
o.
047
tt
+
53-06
u
Solid Phase.
NajCA +Na2SO4.ioH2O
" +Na2S04
EQUILIBRIUM IN THE SYSTEM SODIUM OXALATE, URANYL OXALATE AND
WATER AT 15° AND 50°. (Colani, 1917.)
Results at 50°.
Gms. per 100 Gms.
Sat. Sol. Solid Phase.
Gms. per 100 Gms
Sat. Sol.
Results at 15°.
Solid Phase.
Na2C2O4.
3-09
4-93
I. 80'
0.80
O
U02C204.
o
3.14
5.01
2.65
0.47
Na2C204
" +2.1.2.5
2.1.2.5+2.4.5.11
2.4.5-11 +U02C204.3H20
U02C204.3H20
Na2C204.
4.28
9-03
4.62
3-60
I.OI
o
U02C204.
o
13.09
12.33
9.84
3.58
I
" +2.1.2.5
2.1.2.5+2.2.3.5
2.2.3.5+2.4.5.11
2.4.5-1 1 +UO2C2O4.3H2O
U02.C204.3H20
2.1.2.5 = Na2(U02)(C204)2.5H20, 2.2.3.5
Na2(U02)4.(C204)5.iiH20.
Na2(U02)2(C204)3.5H20, 2.4.5.11 =
SODIUM PALMITATE CH3(CH2)14COONa.
100 gms. sat. solution in H2O contain 0.2 gm. sodium palmitate.
100 gms. sat. solution in 5% aq. bile salts contain I gm. sodium palmitate.
ipo gms. sat. solution in 5% aq. bile salts + i% lecithin contain 2.4 gms.
sodium palmitate. (Moore, Wilson and Hutchinson, 1909.)
SOLUBILITY OF SODIUM PALMITATE IN PALMITIC ACID.
Gms. Na Palmitate
per 100 Gms.
Solid Phase (Na t°.
Palmitate +
Palmitic Acid).
0.7 71
II. 12 72.9
13-78 73-5
16.36 76
18.70 79.2
26.55 82
(Donnan and White, 1911.)
60.2
62
64.4
66.65
67-75
68.95
Gms.
Na Palmitate
per zoo Gms.
Liquid Phase,
2-3
4.96
7.98
12.28
13.72
15.56
Gms.
Na Palmitate
per loo Gms.
Liquid Phase.
22.60
28.65
29.07
30-7
33.36
36.02
Gms. Na Palmitate
per 100 Gms.
Solid Phase (Na
Palmitate +
Palmitic Acid).
25.38
35.05
35-23
35-9
35-66
39.64
The solid phases form three series of solid solutions.
A special apparatus was devised for preparing the saturated solutions and filter-
ing from the solid phases.
SODIUM PHENOLATE
662
SODIUM p NITROPHENOL C6H4.ONa(i).NO2(4).
SOLUBILITY IN WATER AND IN AQUEOUS NORMAL SOLUTIONS OF NON-
ELECTROLYTES.
(Goldschmidt, 1895.)
Cms. C6H4.ONa(i).NO2(4) per 100 Cms. Solution in:
* .
Water.
Alcohol.
Urea.
Glycerine.
Acetone.
Propionitril.
Acetonitril. Urethane.
23-7
5-597
5.6I5
6.244
6.188
6.
225
6.257
6
.065
6.
520
28.6
6.721
6.874
7.489
7.440
7-
498
7-571
7
.328
7-
889
30.6
7.256
.
»
33-6
8.125
8.318
9-000
9.025
9-
025
9.066
8
.886
9-
507
35-9
8.851
.
• .
36.i
8.883
9.683
9.688
9-
665
9.911
9
.667
10.
248
40.2
9.881
10.147
10.666
10.777
10.
695
10.905
10
.667
ii.
379
45-2
".235
11.513
12.068
12.229
12.
869
So. i
12.730
13.133
13.555
13.785
.
,
The
solid phase is C6H4ONa.NO2.4H20
below 36°, and C6H4ONa.
NOt.
2H2O
above
36° in each
case.
•
SODIUM PHOSPHATE (Ortho) Na3PO4.i2H2O.
SOLUBILITY IN WATER.
(Mulder).
« Gms. per 100
1 • Gms. H20.
t°.
Gms. per 100
Gms. H2O.
o 1.5
25
15.5
10 4.1
30
2O
20 II
40
31
50
43
60
80
IOO
Gms. per 100
Gms. H2O.
55
8l
108
SODIUM Hydrogen PHOSPHATE Na2HPO4.i2H2O.
SOLUBILITY IN WATER.
(Shiomi, 1908; Menzies and Humphrey, 1912.)
Gms. NajHPC
)4
t°.
per loo Gms.
Solid Phase.
H20.
-0.43
1.42
Ice
— 0.24
0.70
"
— O.5Eutec.
. . .
"+Na2HP04.i2H20
+0.05'
1.67
Na2HPO4.i2H2O
IO.26
3-55(S)
"
IS-"
5-23(8)
"
2O
7.66
"
25
12
"
30.21
20.81(8)
"
30.76
23.41(8)
"
32
25.7
"
33.04
30.88(8)
M
34
33.8
"
35.2 tr.pt.
' " +Na2HPO4.7H2O
36.45 '
... (S)
«i
37-27
47.5i(S)
NajHPO4.7H2O
39.2
51-8
"
45
67.3
47-23
76.58(8)
48.3tr.pt.
48 "
::: (s)i
50
80.2 N
55.17
81.4 (S)
60
82.9
70.26
88.n(S)
80
92-4
89.74
102.87(8)
90.2
IOI.I
95 tr.pt.
. . .
95.2 "
... (S)
96.2
104.6
99.77
102.15(8)
105
103.3
1 20
00.2
per loo Gms. Solid Phase.
NaaHPO4.7H2O
NajHPO*
Results marked (S) by Shiomi, all others by Menzies and Humphrey.
100 gms. H2O dissolve 12.2 gms. Na2HPO4 at 25°, determined by refractometer.
(Osaka, 1903-8.)
IOO gms. H2O dissolve 5.23 gms. Na2HPO4at 15°, 6?i6= 1.049. (Greenish and Smith, 1901.)
loo gms. alcohol of </i6 = 0.941 dissolve 0.33 gm. Na2HPO4 at 15.5°.
663
SODIUM Dihydrogen PHOSPHATE NaH2PO4.
SOLUBILITY IN WATER.
(Imadsu, 1911-12.)
Cms. NaH2PO4
Solid Phase.
NaH2P04.2H20
SODIUM PHOSPHATES
t°. per 100 Gms.
H20.
O.I
57-86
5
63.82
10
69.87
IS
76.72
20
85.21
25
94.63
30
106.45
35
120-44
40
138.16
40 . 8 tr. pt.
142.55
+NaH2P04.H20
NaH2PO4.H2O
Gms. NaH2PO4
t°. per loo Gms. Solid Phase.
H20.
45
148 . 20
NaH2P04.H,0
50
I58.6I
"
55
170.85
"
57
I75.8I
.«•
57-4tr.
pt. ...
" +NaH2Pl
60
179-33
NaH2PO4
65
184.99
"
69
190.24
"
80
207 . 29
"
90
225.31
if
99.1
246.56
"
SODIUM Acid PHOSPHATE NaH2PO4.H3PO4.
SOLUBILITY IN WATER AND IN ANHYDROUS PHOSPHORIC ACID, DETERMINED
BY THE SYNTHETIC METHOD.
(Parravano and Mieli, 1908.)
Solubility in Water. Solubility in H8PO8.
'Gms. Gms.
NaH2PO4.-
H3P04per
100 Gms.
Sat. Sol.
87.48 NaH2P04
88.65 "
91.47
92.67
95-79
97-99
100
t°.
Gms.
NaH2P04.-
H3PO4per
100 Gms.
Solid Phase. t°.
Sat. Sol.
- 5-7
20.77
Ice 79.7
- 7.9
26.92
85
-11.4
34-15
IOI.7
-38
56.66
104.5
-34
80.46
NaH2P04 1 10
81.82
119
51.7
83.68
126.5
Solid Phase. t°.
98.5
III
"+NaH2P04.H3P04 119
NaH2PO4.H3PO4 122
123
NaH2P04.-
H3PO4per
loo Gms.
Sat. Sol.
52.72
77-55
81.71
87.20
m. pt. of the HaP04 = 40.6"
Data are also given for the fusion points of NaH2PO4 + H3PO4.
Fusion-point data for mixtures of NaPOa + Na4P2O4 are given by Parravano
and Calcagni (1908, 1910.)
EQUILIBRIUM IN THE SYSTEM SODIUM HYDROXIDE, PHOSPHORIC ACID AND
WATER AT 25°.
(D'Ans and Schreiner, igioa.)
Mols. per 1000 Gms. Sol.
Na.
P04.
13-32
4.28
0.040
3-24
0.183
2.24
0.752
2-73
1. 08
3-48
1.33
2.62
1.09
1.56
0.78
2.38
1. 60
3.18
2.24
4-65
3-55
S-63
3.87
6.31
4.63
Solid Phase.
NaOH.H20
NasPO4.i2H2O
NasPO4.i2H2O+Na2HPO4.i2H2O
Na2HP04.i2H20
Na2HP04.7H20
Na.
P04.
— > ouiiu JT uase.
6.76
4.88
Na2HPO4.7H2O
7-31
5.55
" unstable
6.76
4.88
" +NatHPO4.2H2O
6.19
4.68
NajHPO^HjO
6.01
4.67
n
5-i2
4.36
«
4.81
4.22
a
4.36
4.08
a
4.06
4-03
«
4.19
4.38
"
4.32
4.96
u
4.65
5.89
tt
4.88
6.40
M
SODIUM PHOSPHATES
664
SODIUM PyroPHOSPHATE Na4P2O7.ioH2O.
SOLUBILITY IN WATER,
(Mulder; Poggiale.)
O
10
20
Cms. per
100 Cms. H2O.
3-16
3-95
6.23
25
30
40
So
Gins, per
loo Cms. H2O.
8.14
9-95
13.50
17.45
60
80
IOO
Cms. per
zoo Cms. H2O.
21.83
30.04
40.26
SODIUM PyroPHOSPHATES.
SOLUBILITY IN WATER.
(Giran,
Salt.
Monosodium Pyrophosphate
Disodium Pyrophosphate
Trisodium Pyrophosphate
Formula.
NaH3P207
Na2H2P207.6H2O
Na3HP207.6H2O
'AO Gms. Anhydrous Salt
per loo cc. Sat, Sol.
18 62.7
18 14.95
18 28.17
SODIUM PHOSPHITES
SOLUBILITY OF SODIUM PHOSPHITES, ETC., IN WATER.
Salt.
Formula.
Gms. Salt
t°. per loo Gms. Authority.
H,0.
Hydrogen Phosphite
(NaH)HPO3.2iH2O o
56
!(Amat. — Compt.
tt
tt
10
66
rend. 106, 1351, '88.)
u
"
42
*93
Hypophosphate
Na4P2O6.ioH20
cold
3-
3 j
Hydrogen Hypophosphate
Na3HP206.9H20
?
4
5
(Salzer — Liebig's
Tri Hydrogen
u
NaH3P2063H20
cold
6.
7
-/Vim* 2 1 if Xf o2./
Di Hydrogen
Di Hydrogen
u
tt
Na2H2P2O6.6H20
Na2H2P2O6.6H2O
cold
b. pt.
2.
20.
«;
0
(Salzer — Liebig's
Ann. 187, 331, '77.)
Hypophosphite
(NaH)HP02.H2O
25
IOO.
0
(U. S. P.)
Hypophosphite
(NaH)HPO2.H2O
b. pt.
830
100 gms. H2O dissolve 108.7 gms. anhydrous sodium hypophosphite (NaH2PO2)
at 15°, dis of sat. sol. = 1.388. (Greenish and Smith, 1901.)
SODIUM (Double) PHOSPHATE, FLUORIDE Na3P04.NaF.i2H2O.
IOO gms. water dissolve 12 gms. of the double sodium salt at 25°, and 57.5 gms.
at 70°. Sp. Gr. of solution at 25° = 1.0329; at 70° = 1.1091. (Briegleb, 1856.)
SODIUM PICRATE C6H2(NO2)3.ONa.H2O.
SOLUBILITY IN WATER AND IN AQUEOUS SOLUTIONS AT 25°.
(Fisher and Miloszewski, 1910.)
IOO cc. H2O dissolve 4.247 gms. C6H2(NO2)3.ONa.H2O at 25°.
Solubility in Aq. Gms> C6H2(NO2)3.ONa.H2O per 100 cc. Aq. Solution of Normality:
Solution of:
O.OI.
O.O2.
0.04.
0.066.
O.IO.
0.25.
0.5.
I.
Na2C03
4.159
4.044
3
.807
3-
434
3.187
2
.017
I.I2O
0.611
NaCl
4.189
3.956
•677
3.
335
3.021
I
.678
0.846
0.410
Na2S04
4.246
4.102
3
.879
3-
651
3.195
2
.053
I.I56
0-552
Na3PO4
4.235
4.051
3
.814
3-
562
3.225
2
.219
1.329
0.705
NaOH
4.192
4.048
3
.715
3-
339
2.941
X
.781
0.921
0.371
NaNO3
4.154
4.029
3
.710
3-
363
3.041
I
-932
0-943
0.684
NaBr
4.190
4.II7
3
.770
3-
384
3.024
I
•777
0.912
0.499
Data for the solubility of sodium picrate and the sodium salts of other nitro-
phenols in aqueous alcohol and acetone solutions at 25° are given by Fisher (1914).
Wt. Per cent
CzHjOH in
Solvent.
dx of
Sat. Sol.
Gms. CeB^OH-
COONa per 100
Gms. Sat. Sol.
Wt. Per cent
QH6OH in
Solvent.
da, of
Sat. Sol.
O
1.256
53-56
60
1. 066
10
1-235
52.10
70
1.016
20
1.205
50.20
80
0-957
30
1.176
48
90
0.885
40
1.142
45-50
92.3
0.864
50
1.106
42.20
IOO
0.805
66s SODIUM SALICYLATE
SODIUM SALICYLATE C6H4.OH. COONa.
SOLUBILITY IN AQUEOUS ETHYL ALCOHOL AT 25°. (Seideii, 1909, 1910.)
Gms. CgEUOH-
COONa per 100
Gms. Sat. Sol.
38.40
33
25
15
12
3-82
100 gms. sat. solution in water contain 51.8 gms. C6H4OHCOONa at 15° and
du of the sat. sol. is 1.249. (Greenish and Smith, 1901.) See also last line of first table
on p. 590.
100 gms. propyl alcohol dissolve 1.16 gms. C6H4OHCOONa at ord. temp.
(Schlamp, 1894.)
Sodium salicylate distributes itself between olive oil and water at 15° in the
ratio of 0.156 gm. C6H4OHCOONa per 100 cc. oil layer and 1.444 gms. per 100 cc.
aqueous layer. (Harrass, 1903.)
SODIUM SELENATE Na2SeO4.ioH2O.
SOLUBILITY IN WATER. (Funk, igooa.)
Gms. Mols. Gms. Mols.
to Na2Se04per Na2SeO4per Solid to Na2SeO4 per Na2SeO4 per Solid
100 Gms. loo Mols. Phase. 100 Gms. 100 Mols. Phase.
Solution. H2O. Solution. H^.
O 11-74 I-26 NaaSeOi-ioHaO 35.2 45-47 7-94 NaaSeO*
15 25.01 3.18 39.5 45.26 7.87
18 29.00 3.90 50 44.49 7-63
25-2 36-91 5-57 75 42-83 7.14
27 39.18 6.13 100 42.14 6.93
30 44.05 7.50
Sp. Gr. of saturated solution at 1 8° = 1.315.
SODIUM [SILICATE Na2SiO3.9H2O.
SOLUBILITY IN AQUEOUS SODIUM HYDROXIDE AND SODIUM CHLORIDE
SOLUTIONS. (Vesterberg, 1912.)
Gms. per 100 cc. Sat. Solution.
Solvent. t°. dtt of
Sat. Sol. NaaO. SiO2 = NajSiOs.gHzO. NaCl.
Approx. 0.5 n NaOH 17.5 1.129 6.942 5.419 =25.56
NaCl 17.5 1.150 7.347 7.172 33.83 2.297
^Saturated NaCl Solution 19 1.258 4.563 4.376 20.64 27.91
~ Solid phase Na2SiO3.9H2O in each case.
Fusion-point data for Na2SiO3 + SrSiO3 are given by Wallace (1909). Results
for Na2SiO3 + Na2WO4 are given by van Klooster (1910-11).
SODIUM STANNATE Na2SnO3.3H2O.
100 gms. H2O dissolve 67.4 gms. at o°, and 61.3 gms. at 20°. Sp. Gr. of solution
at 0° = 1.472; at 20° = 1.438. COrdway, 1865.)
SODIUM SUCCINATE (CH2)2(COONa)2.6H2O.
SOLUBILITY IN WATER. (Marshall and Bain, 1910.)
Gms. (CH2)r Gms.
•
«•• per, S°M Phase.
H20. H20.
O 21.45 (CH2)2(COONa)2.6H20 50 56.3 (CH2)2(COONa)2.6H2O
I2.S 27.38 62.5 78.49
2$ 34.90 64.9 83.38 " +(CH2)2(COONa),
37-5 43.64 75 86.63 (CHMCOONa),
SODIUM SUCCINATES
666
o
2-5
25
37-5
SOLUBILITY OF SODIUM HYDROGEN SUCCINATE IN WATER.
(Marshall and Bain, 1910.)
Cms. (CH^y
(COOH)(COONa) Solid Phase,
per 100 Cms. H2O.
NaHSu*.3H2O
Cms. (CH2)2-
(COOH)(COONa)
17-55
27-93
39.82
60. 01
Solid Phase,
per loo Cms. H2O.
38.7 63 . 99 NaHSu.3H2O +NaHSu
50 67.37 NaHSu
62-5 76.15
75 86
EQUILIBRIUM IN THE SYSTEM SODIUM SUCCINATE, SUCCINIC ACID AND WATER.
(Marshall and Bain, 1910.)
Results at o°.
Gms. per too Gms.
Sat. Sol.
NaaSu.
H2Su.'
O
2.68
H2Su'
3-23
4-76
"
5.38
5-83
"
8.27
7.12
" 4
8.67
6.27 Na]
asu.3i
9.68
4-74
«
11.74
3-49
"
15.62
2-34
«
18.36
1.90
" 4
18.07
1.67
Na,
17.87
0.94
17.64
Results at
50°.
0
19.27
H2Su'
5-95
22.90
"
10*25
25-33
ii
15.49
28.73
"
19.65
31-73
"
20.72
26.51 NaHSu
22.53
18.44
«
25-53
13.09
*
28.28
9.46
"
30.48
7.38
ii
37-33
4.20
36.85
3-88
Na,
36.67
2.66
36.43
0
Solid Phase.
+NaHSu.3H2O
+Na2Su.6H20
+NaHSu
+Na2Su.6H20
' The following double and triple points were located :
Results at
25°.
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
NajSu.
H2Su.
0
7.71
H2Su
3-68
10.26
"
8.99
13-35
*
12.64
15-53
"
15.26
16.90
" +NaHSu.3H,O
15.97
13 . 83 NaHSu.3H2O
18.89
8.41
"
22.71
5-65
"
26.88
4.08
" +Na2Su.6HaO
26.50
2.38
Na2Su.6H2O
26.11
0.85
"
25.87
O
"
Results at
75°.
0
37-64
H2Su
8.22
40.38
"
13.14
42.50
"
16.93
44.38
«
19.56
45-98
" 4-NaHSu
21.88
35-6o
NaHSu
24.30
26.82
"
29-45
15.28
"
36.11
7-79
"
41.26
4-93
"
45-27
4
" +Na2Su.H20
45-36
3-17
NazSu.HaO
45-93
1.23
"
46.42
0
'
34.9
37-8
38.7
63.4
64.9
Gms. per 100 Gms. Sat. Sol.
5.6
25.46
16.44
3.64
30.8
19.6
22.47
42.92
45-43
Solid Phase.
NaHSu.3H2O +NaHSu H-N^Sn.
NaHSu.3H20 +NaHSu+H2Su
NaHSu.3H2O+NaHSu
Na,Su.6H2O+Na2Su.H2O4-NaHSu
*In the above tables the abbreviation Su is used for (CH2)2(COO)2.
667
SODIUM SULFATE
SODIUM SULFATE Na2SO4.
SOLUBILITY IN WATER.
(Mulder; Lowel, 1851; Tilden and Shenstone, 1883; Etard, 1894; Funk, igooa; Berkeley, 1904.)
Gms. Na2SO4 per
t°. 100 Gms. j;
Mols.
fa2SO4pe:
Solution.
Water/
Liter (B.;
0
4.76
5-o
0.31 :
5
6.0
6.4
10
8-3
9-0
0.631
15
n. 8
13-4
20
16.3
19.4
1.32
25
21.9
28.0
27
•5 25.6
34-o
. . .
30
29.0
40.8
2.63
31
30.6
44.0
32
32-3
47-8
32
•75 33-6
50.65
3.II
33
33-6
50.6
35
33-4
50.2
40
32.8
48.8
3.01
Na2SO4
Gms. Na2SO4
t°. too Gms.
per
]
Mols.
*a2S04p
Solution.
Water. Liter (I
50
3i
.8
46
•7
2 .92
60
31
.2
45
•3
2.83
80
3o
•4
43
•7
2.69
100
29
.8
42
•5
2.6o
120
29
•5
41
•95
I4O
29
.6
42
160
30-7
44
•25
230
3i
•7
46
•4
o
16
.3
19
•5
5
19
•4
24
10
.23
.1
30
15
27
•o
37
20
30
.6
44
25
34
.6
53
...
Na»SO«
Na2S04.7HjO
The very carefully determined values of Berkeley are as follows:
Gms.
dtoi
Sat. Sol.
Na2SO4 pe
100 Gms.
H20.
0.70
[.0432
4.71
10.25
.0802
9.21
15.65
.1150
14.07
20.35
.1546
. . .
24.90
.2067
27.67
27.65
•2459
34-05
30.20 ]
[.2894
41.78
31.95 ]
[.3230
47.98
Gms.
dt of Na,jSO4 per
Sat. Sol. 100 Gms.
H20.
Solid Phase.
32.5tr.pt.
33-5
38.15
44.85
60. 10
75.05
89-85
[oi . 9*
* B. pt.
3307
3229
3136
2918
2728
2571
2450
49.39
48.47
47-49
45-22
43-59
42.67
42.18
Na2SO4.ioH2O+NajSO4
NasSO,
The following additional data at high temperatures, determined by the sealed
tube method, are given by Wuite (1913-14).
t°
Mol.
Per cent
Gms.
Na2SO4 per
Na2SO4.
IOH2OmS
62
5.39
44-92
70
5-27
43.87
80
5.18
43-07
1 2O
5.04
41.84
190
5-255
43.74
192
5-27
43.87
Solid Phase.
NazSO, (rhombic)
Mol.
t°. Per cent
Na^SO,.
Gms.
NajSO, per
100 Gms.
H20.
208 5.39
44.92 ]
235tr.pt.
241 5-39
250 5.04
279 4.12
319 2.56
44.92
41.84
33.84
20.71
Solid Phase.
(rhombic)
" +monoclinio
monoclinic)
Supersolubility curves for the ice phase, Na2SO4.7H2O phase and Na2SO4 phase
were determined by Hartley, Jones and Hutchinson (1908) by agitating mixtures
of sodium sulfate and water contained in sealed tubes, and noting the points at
which spontaneous crystallization occurred while the tubes were gradually cooled.
The effect of mechanical friction, produced by bits of glass, garnet, etc., was also
studied.
SODIUM SULPATE 668
SODIUM SULFATE
SOLUBILITY OF MIXTURES OF SODIUM SULFATE AND MAGNESIUM SULFATE
IN WATER (ASTRAKANITE) Na2Mg(SO4)24H2O.
(Roozeboom, 1887, 1888.)
Solid
Phase.
Astrakanite
Astrakanite + NajSO4
Astrakanite + MgSO4
Mols.
per 100
Grams per 100
«;».
Mols.
H20.
Grams
HaO.
fra2SO4. MgSO4.
Na2S04.
Mgso4:
22
2
•95
4
.70
23
•3
31
•4
24
•5
3
•45
3
.68
27
.2
24
.6
30
3
•59
3
•59
28
•4
24
.1
35
3
.71
3
.71
29
•4
24
.8
47
3
.6
3
.6
28
•4
24
.1
22
2
•95
4
.70
23
•3
31
•4
24
•5
3
•45
3
.62
27
.2
24
.2
30
4
•58
2
.91
36
.1
19
.1
35
4
•3
2
.76
33
•9
18
•44
18
•5
3
.41
4
.27
45
•5
22
2
•85
4
•63
35
.2
48
•9
24
•5
2
.68
4
.76
32
•5
5°
.3
30
2
•3
5
.31
25
•9
55
• o
35
I
•73
5
.88
23
•5
59
•4
SOLUBILITY OF MIXTURES OF SODIUM SULFATE, POTASSIUM CHLORIDE,
POTASSIUM SULFATE, ETC., IN WATER.
(Meyerhoffer and Saunders, 1899.)
*- o
Sp. Gr. of
Mols. per 1000 Mols. H2U.
*
Solutions.
SO, K9
Na2
C12
*4-
4
5-
42
14.
39
5I-83
60.
8
K3Na(SO4)2+Na2SO4.ioH2O-r-
0.
2
3-
35
12.
78
50-
93
60.36
Na2S04.ioH2O+KCl+NaCl
— 0.
4
3-
59
16.
38
40-75
53-
54
Na2S04.ioH20+KCl+K3Na(SO4)2
16.
3
4-
72
17-
58
50.
56
63.42
K3Na(S04)2+KCl+NaCl
24-
8
1.2484
4-
37
20.
oo
48.
36
64.
01
K3Na(SO4)2+KCl+NaCl
*i6.
3
16.29
9-
16
61.
06
53-
93
K3Na(S04)2+NaCl-i-Na2SO4.ioH2O+
Na2SO4
24.
5
1.2625
14.
45
9-
90
58.
46
53-
91
K3Na(S04)2+NaCH-Na2SO4
0.
3
2.
75
25-
77
17-
93
40.
95
K3Na(SO4)2+KCl+K2SO4
25-
o
1.2034
2.
94
36.
20
14.
80
48.
06
K3Na(SO4)2+KCl+K2SO4
*i7-
9
1.2474
13-
84
0.
0
62.
57
48.
70
Na2SO4.ioH20+Na2SO4+NaCl
i
1 . 2890
IO.
08
40.
33
0.
0
K3Na(SO4)2+Na2SO4.ioH2O+Na2SO4
— 21.
4
...
..
.
..
.
46.
61
46.
36
NaCl.2H2O+Na2SO4.ioH2O
-23.
7
.
10.
51
39-
58
09
NaCl.2H2O+KCl
— 10.
9
I.
45
30.
68
29.
23
KC1+K2SO4
- 3
16.
25
IO.
03
6.
21
K3Na(SO4):r|-Na2SO4.ioH2O
- 3
16.
24
10.
03
6.
21
.
K3Na(S04)2+K2S04
-14
i.
39
25-
59
8.
78
32-
94
KsNa(SO4)iH-Na2SO4.ioH2O-|-KCl
-14
i.
39
25.
59
8.
78
32-
94
K3Na(SO4)2+K2SO4+KCl
-23.
3
...
o.
4i
15.
15
44.
20
58.
97
Na2SO4.ioH2O+KCl+NaCl.aH2O
* Indicates transition points.
669
SODIUM SULFATE
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
ACETATE AT 25°.
(Fox, 1909.)
Gms. per 100 Gms. Sat.Sol.
Solid Phase.
Gms. per too Gms. Sat. Sol.
Solid Phase.
' CHjCOONa.
Na2SO4.
CH3COONa.
j^ajSO4.
0
21-9
NasS04.ioH20
12.58
I3-50
Na,SO4.ioH,O
4.10
17.72
"
16.26
II .50
"
7.71
16.48
H
20.68
8.10
it
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS SODIUM CHLORIDE AT 15°.
((Schreinemakers and de Baat, 1909.)
Gms. per 100 Gms. Sat. Sol.
NaCl.
Solid Phase.
Gms* per 100 Gms. Sat. Sol.
5-42
11-51
15-97
7.86
5-87
5-23
NajS04.ioH20
NaCl.
21.03
23-39
25.21
NajSO,.
5.26
Solid Phase.
Na2S04.ioH,0
5.64 " +NaCl
2 . 26 NaCl
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT DIFFERENT TEMPERATURES.
(Seidell, 1902.)
Results at 10°.
Results at 21.5°.
Results at 27*
Sp. Gr.
of
Gms. per too Gms.
H20.
Sp. Gr.
of
Gms. per 100 Gms.
H20.
Sp. Gr.
of
Gms. per 100 Gms.
HzO.
Solutions. NaCl.
Na2SO4.
Solutions.
Nad.
Na2SO4.'
Solutions.
NaCl.
Naa
S04.
1. 080
o.o
9-
14
I
164
O-O
21-33
1.228
o.o
31-
10
1.083
4.28
6.
42
I
169
9-05
15.48
1.230
2.66
28.
73
I .IO2
9.60
4-
76
I
199
17.48
13-73
1.230
5-29
27.
17
I.I50
I5-65
3-
99
I
.214
20.41
13.62
1-235
7.90
26.
02
1.164
21.82
3
97
I
•243
26.01
15-05
1.259
16.13
24.
83
I .192
28.13
4
I
.244
26.53
14.44
1-253
18.91
21.
39
I .207
30.11
4
34
I
•244
27-74
13-39
1.249
19.64
2O.
ii
I .217
32.27
4
59
I
.244
31-25
10.64
1.245
20.77
19.
29
1.223
4
75
I
•243
31.80
10.28'
1.238
32-33
9-
53
I
•245
32.10
8.43
I
.219
33-69
4-73
I
.212
34.08
2-77
I
.197
35-46
o.oo
Results at 30°.
Results at
33°.
Results at
35°.
Sp. Gr.
of
Gms. per 100 Gms.
HizO.
Sp. Gr.
of
Gms. per 100 Gms.
H?0.
Sp. Gr.
of
Gms. per 100 Gms.
Solutions.
NaCl.
Na2S04.
Solutions.
NaCl.
Na2SO4.
Solutions.
NaCl.
Na2SO .
I.28l
o.o
39
.70
I
•329
o.o
48.48
1.324
o.o
47
94
1.282
2.45
38
•25
I
•323
1.22
46.49
«-3«4
2.14
43
•75
1.284
5-6i
36
I
.318
1-99
45.16
1.256
13-57
26
.26
I .290
7.91
35
:96
I
•3r5
2.64
44.09
1.238
18.78
19
74
1.276
10. 61
31
.64
•309
3-47
42.61
1.231
71 . OI
8
.28
1.270
12.36
29
-87
•265
12.14
29.32
i-i93
3 ? - 63
o
.00
1.258
15-65
25
.02
•237
21.87
16-83
1.249
18.44
21
•30
•234
32.84
8.76
1.244
20.66
19
.06
.217
33-99
4.63
1.236
32-43
9
.06
I
.208
34-77
2-75
SODIUM SULFATE
670
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
CHLORIDE AT 25°.
(Cameron, Bell and Robinson, 1907.)
^ Of Gms. per 100 Gms. H2O.
Sat. Sol. .'
I.2I73
I.2l62
I.2I50
1.2275
1.2385
1.2571
1.2476
NaCl.
2.96
5-79
9.90
13-43
15-82
19-13
23.22
NazSO,.
26.60
24.32
21.41
19.62
19.64
20.73
16.28
Solid Phase.
Na2SO4.ioH2O
Sat. Sol.
NaCl.
Na,S04.
ouiiu i nase.
.2429
26.54
12.64
Na2S04
.2438
31.06
9.98
"
•2451
32.41
9-93
"
•2453
33
9-84
" +NaCl
.2309
33-81
6.66
NaCl
.2162
34.60
3.38
"
.2002
35.8o
0
"
Data are also given for the ^ystem sodium sulfate, sodium chloride, calcium
sulfate and water at 25°.
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
HYDROXIDE AT 25°.
(D'Ans and Schreiner, 1910.)
Mols. per 1000 Gms. Sat. Sol.
Mols. per looq Gms. Sat. Sol.
(NaOH)2. NajSCv
0.074 1.41
0.70 1. 08
1-47 0.90
2.02 0.59
Solid Phase.
NasSO,
(NaOH)2.
2.82
3-52
5.83
6.62
Na,S04.
0.24
0.126
0.013
O
Solid Phase.
Na,SO«
NaOH.H20
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 25°.
(D'Ans, 1906; 19090; 1913.)
Mols. per
looo Gms.
Sat.
Sol.
Solid Phase.
H2S04.
Na2S04.
0
I.54I
Na2S04.ioH20
0.286
1.671
"
0.338
1.742
i<
O.6o
1.85
"
0.763
2
"
0.884
2.256
4-NajJ
0.423
0.77
NaHSO4.H2O
0.496
0.47
"
1.666
2-437
Na2SO4+Na3H(SO4)2
1.576
2.363
" +Na3H(SO4)2.H2O
2.611
2.091
Na3H(S04)2+ "
5-91*
0.409
NaHSO4
6.30
0.332
«
6.64
0.297
" +NaH3(S04)2.H20
6.90
0.173
NaH3(S04)2.H20
7.36
O.07I
"
7-74
0.047
«
8.12
0.037
«
8.40
0.046
"
Mols. per 1000 Gms.
Sat.
Sol.
Solid Phase.
S03.
Na2SO4.
8.70
0.076
NaH3(SO4)2.H2O
8.86
0.156
"
8.93
0.273
"
8.84
0.527
" (unstable)
8.70
0.8o8
" "
8.62
0.844
" "
8.61
0.899
"
8.87
0-445
• " +Na,S04.4*H2S04
8-93
0-437
Na2S04.4|H2S04
9.08
0-394
"
9-36
0.425
" +NaHS20,
9.18
0.567
NaHSjiO,
9.42
0.728
"
9.48
0.76
"
9.48
0-953
" +?
9-85
0.787
?
9.98
0.908
?
9.77
1.03
unstable
10. 16
0.797
10.78
0.302
' From this point on the figures in this column are Mols.SO3 = H2SO4 + S03.
loo cc. sat. solution of Na2SO4 in absolute H2SO4 contain 29.99 gms. Na2SO4
and the molecular compound which is formed contains 8 mols. H2SO4 per I mol.
Na2SO4 and melts at about 40°. (Bergius, 1910.)
Aqueous H2SO4 containing 0.51 mol. per liter dissolve 2.238 mols. Na2SC>4 per
liter at 25°; Aq. H2SO4 of 0.779 mol- per liter dissolves 2.465 mols. Na2SO4 at the
same temperature. (Here, 1911-12.)
671
SODIUM SULFATE
SOLUBILITY OF SODIUM
SULFATE IN AQUEOUS ETHYL ALCOHOL.
(de Bruyn, 1900.)
r.
Concentra-
tion of
Alcohol in
Wt. %.
Gms. NajSO4
per too Gms.
Aq. Alcohol.
IS
0
12.7
9.2
6-7
"
19.4
2.6
II
39-7
o-5
"
58.9
O.I
(I
72
0
M
0
37-4
"
II. 2
16.3
"
20.6
7
II
30.2
2
25
0
28.2
ti
10.6
13-9
tt
24
4-5
ft
54
0.4
36
0
49-3
8.8
29.2
"
12.8
22.4
II
17.9
15-4
II
18.1
15-3
II
28.9
5-4
II
48.7
0.8
45
o
47-9
*'
9
27-5
ii
14-5
19.2
"
20. 6
12.3
Gms.
per 100 Gms.
Solution.
bond Phase.
HA
CiH6OH.
Na2S04.
88.7
0
11.3
NajSO4.ioH,O
85.1
8.6
6-3
• «
78.6
18.9
2.5
«
60
39-5
0-5
«
4I.I
58.8
O.I
»
28
72
0
«
72.8
o
27.2
Na.S04.7HA
76.5
9-5
14
74-3
19.2
6.5
M
68.4
29.6
2
«
78.I
o
21.9
Na,SO4.ioH,O
78-5
9-3
12.2
"
72.8
22.9
4-3
"
45-6
54
0.4
" +Na2S04
67
0
33
NaaSO,
70.6
6.8
22.6
"
71.2
10.5
I8.3
"
71.1
15-5
13-4
"
71
15-7
13-3
"
66.5
28.4
"
50-9
48.3
o.S
ti
67.6
0
32.4
"
71 3
7- I
21.6
«
71.8
12. I
16.1
«
70.6
18.4
IO
"
65-6
29.5
4.9
"
The
and de
25
following additional determinations at 25° are given by Schreinemakers
Baat (1909):
63.41 34.84 1.75 Na2S04.ioHI0
... 49 50-5
46.6
34*9
53
64-95
1-75
0.5
0.4
0.15
+Na,S04
NajSO,
Between certain concentrations of the aqueous alcohol the liquid separates into
two layers. The following results were obtained at 25°, 36° and 45°:
Upper Layer.
Lower Layer.
Gms.H20. Gms.C2H5OH
. Gms.Na2SO4.
Gms.H2O. Gms.C2H6OH
. Gms.Na2SO4.
25
66.5
27-3
6.2
67.4
5-1
27-5
n
68.1
23-9
8.0
68.5
6.0
25-5
tt
68.3
23.1
8.6
68.3
6.7
25.0
36
. . .
. . .
66.6
4.1
29-3
«
57-7
38-4
3-9
M
65.0
28.3
6.7
68.8
5-9
25-3
II
68.1
21 .2
10.7
68.9
9-4
21.7
45
61.8
32-9
5-3
ii
65.8
25-3
8.9
68.4
8.8
22.8
tt
66.0
24. Q
10. 0
68.6
10. 1
21-3
Data for equilibrium in the system Na2SO4 + NaCl + C2H5OH + H2O at 15°,
25° and 35° are given by Schreinemakers and de Baat (1909), and Schreinemakers
(1910).
SODIUM SULFATE
672
SOLUBILITY OF SODIUM SULFATE IN AQUEOUS PROPYL ALCOHOL AT 20°.
(Linebarger, 1892.)
Gms.
per ioo Gms.
Alcohol-Water
Mixture.
Gms. Na2SC>4
per ioo
Gms. Sat.
Solution.
1-99
Gms. C3H7OH
per 100 Gms.
Alcohol-Water
Mixture.
Gms. Na2SO4
per ioo
Gms. Sat.
Solution.
42.20 1-99 50.57 0.55
49-77 I-I5 60.64 0-44
55.65 0.72 62.8l 0.38
ioo gms. H2O dissolve 183.7 gms- sugar + 30.5 gms. Na2SO4 at 31.25°, or ioo
gms. sat. solution contain 52.2 gms. sugar + 9.6 gms. Na2SO4. (Kohler, 1897.)
ioo gms. 95% formic acid dissolve 16.5 gms. Na2SO4 at 19°. (Aschan, 1913.)
SOLUBILITY OF SODIUM SULFATE IN AN AQUEOUS SOLUTION OF UREA.
(Lowenherz, 1895.)
Solvent.
ioo gms. H2O+i2 gms. urea
Gms.
Na2SO4 per
The Corresponding Fig-
ure for the Solubility
t.
ioo Gms.
Sat. Sol.
of Na2SO4 in Pure Water
Was Found to be:
20.86
22.36
. . .
24-83
21.21
21.62
28.32
26.50
26.48
29.83
28.23
31.90
32.34
34.85
27-73
33.09
39-92
27.19
32.58
Fusion-point data for Na2SO4 + KC1 are given by Sackur (1911-12). Results
for Na2SO4 + SrSO4 are given by Calcagni (191 2- 1912 a). Results for Na2SO4
+ Na2WO4 are given by Boeke (1907).
SODIUM BiSULFATE NaHSO4. (See also last table, p. 670.)
ioo gms. H2O dissolve 30 gms. NaHSO4 at 16°. (Aschan, 1913.)
ioo gms. H2O dissolve 28. 6 gms. NaHSO4at 25° and 50 gms. at 100°. (U.S.P.VIII.)
ioo gms. 95 per cent alcohol dissolve about 1.4 gms. NaHSO4at 25°. (U.S.P.VIII.)
ioo gms. 95% formic acid dissolve 30 gms. NaHSO4 at 19.3°. (Aschan, 1913.)
SODIUM SULFIDE Na2S.9H2O.
SOLUBILITY IN WATER.
(Parravano and Fornaini, 1907.)
Gms. NajS
per ioo Gms.
Sat. Sol.
— lOEutec. 9.34
Solid Phase.
+ 10
15
18
22
28
32
37
45
50
pt.
13-36
14.36
15-30
16.20
17-73
19.09
20.98
24.19
28.48
Gms. NasS
t°.
per ioo Gms.
Sat. Sol.
60
29.92
70
3I-38
80
33-95
90
37-20
48
tr. pt.
50
26.7
60
28.1
70
30.22
80
32.95
90
36.42
91
.5tr.pt. ...
Solid Phase.
+Na2S.sJH20
JO 28.48 NajS.siHzO 9I.5tr.pt. ... " +NajS.si
Fusion-point data for Na2S + S are given by Thomas and Rule (1917).
SODIUM Antimony SULFIDE. See Sodium Sulfoantimonate, p. 627.
673
SODIUM SULFITE
SODIUM SULFITE Na2SO3.
t°.
0.76
Cms. NajSOs
per ioo Gms.
H20.
2.15
1-37
1.96
4-21
6.24
2.77
3-5*
9.44
12.48
4-5
17.91
1.9
2
5-9
10.6
13.09
14.82
17.61
2O. OI
SOLUBILITY IN WATER.
(Hartley and Barrett, 1909.)
Solid Phase.
Ice
1 +Na2S03.7H20
Ice (unstable)
Gms. N^SOs
t°.
per 100 Gms.
Solid Phase.
H20.
18.2
25-3I
Na2S03.7H20
23.5
29.92
" (unstable)
29
34-99
« «
37-2
44.08
« «
21. 6f
" +Na,SO,
37
28.04
Na,SO,
47
28.13
H
55-6
28.21
«
59-8
28.76
«
84
28.26
"
t tr. pt.
* Eutec.
Oxidation was prevented by preparing the material and making the solubility
determinations in an atmosphere of hydrogen.
Supersolubility curves for the salt are also given.
The Sp. Gr. of the sat. solution at 15° is I.2I. (Greenish and Smith, 1901.)
SODIUM HydroSULFITE Na2S2O4.
SOLUBILITY IN WATER, (jeliinck, 1911.)
Solid Phase.
Gms. NajSA
per 100 Gms.
H20.
19 Ice+Na2S204.2H20
22 (±5% error) Na2s2o4.2H2o
27.8 " +Na2S204
24.1 Na2S2O4 (unstable)
The pure sample was prepared by salting out the commercial product with
NaCl. It is very easily oxidized to Na2S2O5 and must be kept in an indifferent
atmosphere or a vacuum. A special apparatus was required for the freezing-point
determinations (ice curve) and for the solubility determinations. Great difficulty
was experienced in obtaining concordant results with a given sample of
Gms. NajSA <.,.,
*° periS$;n8' Phase.
t°.
— O.IO7
0.394 Ice
— 4.58 Eutec.
— I.IO
4
+ 20
— 2.21
9
52 tr. pt.
-3-15
13
20
-4.17
17
SODIUM SULFONATES
SOLUBILITY IN WATER.
Salt.
Sodium:
2.5 Diiodobenzene Sulfonate
Formula.
Gms.
O Anhydrous
' Salt per ioo
Gms. H2O.
Authority.
3-4
0 Naphthalene Sulfonate
<( <(
2 Phenathrene Sulfonate
~ « it
10 "
Phenol Sulfonate
1.019.
C6H3I2S03Na.H2O
Ci0H7.SO3Na
u
Ci4H9S03Na.|H20
Ci4H9SO3Na.H2O
Ci4H9.SO3Na.2H2O
22.5
22.5
23-9
25
20
20
20
(Boyle, 1909.)
6.82
3-47
6.04
5.87*
0.42
i.i
1.63
14- 7t
IQ. 2%
K = I.067. t <*25 =
SOLUBILITY OF SODIUM /3 NAPHTHALENE SULFONATE IN AQUEOUS HYDRO-
CHLORIC ACID AT 23.9°. (Fischer 1906.)
Normality of Aq. HC1. i.o». 2 n. 3 n. 5 n.
Gms.CioHT.SOsNaperioogms. Aq.HCl 6.47 5.35 4.13 2.42
25
(Fischer, 1906.)
(Witt, 1915.)
(Sandquist, 1912.)
(Greenish & Smith,'oi.)
(Seidell, 1910.)
1.079
SODIUM SULFONATES
674
SOLUBILITY OF SODIUM PHENOL SULFONATE IN AQUEOUS ALCOHOL AT 25°.
(Seidell, 1910.)
Wt. Per cent j r Gms. CsILXOH). Wt. Per cent
CjHiOH in
Solvent.
o(=H20)
10
20
30
40
50
ms. Sat. Sol.
19.38
17.4
15-5
13-6
ii. 7
9-7
rtveat.
60
70
80
90
95
100
d nf Gms. CjEUCOH)
Sa? Sol SO3Na.2H20 per
loo Gms. Sat. Sol.
0.919
0.886
7-5
0.852
0.820
2.9
i.i
0.810
0.8
0.800
i.S
1.079
1.054
1.030
1.004
0.977
In "the ioo per cent C2H6OH solution, the solid phase, C6H4(OH) S03Na.2H2O,
became opaque.
ioo gms. H2O dissolve 18.25 gms. C6H4(OH)SO3Na.2H2O at 14.8°, du.& of sat.
sol. = 1.0675. (Greenish and Smith, 1901.)
SODIUM TARTRATES
SOLUBILITY IN WATER.
Gms. Salt
Salt. Formula. t°. per ioo
Gms. H2O.
Sodium Neutral Inactive Pyrotartrate C6H6O6.Na2.6H2O 20
Dextro 20
Sodium Dihydroxy Tartrate C4H4O8Na2.3H2O o
SODIUM TELLURATE Na2TeO4.2H2O.
ioo gms. H2O dissolve o.f 7 gm. Na2TeO4 at 18°, and 2 gms. at 100°.
phase Na2TeO4.2H2O.
ioo gms. H2O dissolve 1.43 gms. Na2TeO4 at 18°, and 2.5 gms. at 50°. Solid
phase Na2TeO4.4H2O. (Mylius, 1901.)
SODIUM THIOSULFATE Na2S2O3.5H2O(I).
SOLUBILITY IN WATER. (Young and Burke, 1904, 1906.)
Authority.
39.73 (Schlossberg, 1900.)
41.10 "
0.039 (Fenton, 1898.)
Solid
Gms. NazS-A per
i°Jf. ioo Gms. gelid Phase. t°.
Gms. NajSA per
ioo Gms.
Solid Phase.
Sat. Sol.
Water.
Sat.
Sol.
Water.
O
33-
40
50
. l5NaaS2O3.sH2O(I)
0
60.
47
153
Na
iSA-HjOdD
10
37-
37
59
.66 "
IO
61.
04
156.
7
"
20
41.
20
70
.07 "
2O
62.
ii
163.
9
**
25
I43>
15
75
.90 "
25
62.
73
168.
3
a
35
47-
71
91
.24 "
30
63-
56
174.
4
**
45
55-33
123
.87 "
40
65.22
187.
6
**
48.
17* -.
.
. .
. "+Na2S203.2H20(I)
50
66.
82
201.
4
it
.
o
52.
73
in
.6oNa2S203.2H20(I)
56.5*
.
. . .
«*
+Na,SA
10
53-
94
117
. 10 "
0
46.
14
85 . 67 NajSjOa-GHjOdllandlV)
20
55-
IS
122
.68 "
IO
66
106.
8
**
25
56.
03
127
•43 "
13
54-
96
122
«
30
57-
13
138
.84 "
14.35*
«
+Na2S2O3.fH2O.(IV)
40
59-
38
146
.20 "
14.3*
. .
. . .
u
+Na2S203.7H20(III)
50
62.
28
165
.11
o
57-
42
134-
8 Na,SA.7H20(III)
60
65-
68
191
•30 . "
IO
58.
28
139-
7
"
66.
5* .-
.
. . "+Na,SA
20
59.28
145.6 ••
o
41.
96
72
.3oNa2S203.SH20(ID
25
60.
18
I
«
10
45-
25
82
•65 "
30
60.
78
155
*
20
49.
38
97
•55 "
40
62.
60
I67.
4
*•
25
52-
15
108
.98 '«
47-5
64.
68
i
«
30
56.57
130
.26 "
48.5*
. . .
r-
+Na2S203.H20(IID
30.22* ...
, . "+Na2St03.4H20(ID
47-5
64.'
78
l83.9Na2S203.H20(IID
33-
5 58.
59
141
.48Na2S203.4H20(II)
65.
3
188.
2
«
36.
2 60.
5*
153
•23 "
55
66.
45
198.
I
*
36.
6 62.
80
168
.82 "
60
68.
07
213.
I
*
40.
65*..
. .
.
"+Na2SJOa.H20(II)
61*
M,
-f-^SA
* tr.pt.
675
SODIUM THIOSULFATE
SOLUBILITY IN WATER (Continued).
Cms. Na
2SA per
Gms. NajSjOs
per
t".
100 (
jins.
Solid Phase. t°.
100 1
Lrms.
, Solid Phase.
Sat.
Sol.
Water.
Sat.
Sol.
Water.
O
57
•63
136
Na2S203.iH,0(IV) 30
63-
34
172
.80
Na2S20,.H10(V)
10
58
.49
I4O.
9
40
64.
75
183.70 «
2O
59
•57
147-
3
50
66.
58
199
.2
«
25
60
•35
152.
2
55
67.
59
208
•5
"
30
61
•03
156.
6
43*
"+NasS203.*H20'(V)
40
62
•95
I69.
9
" . 25
64*.
21
179
•4
Na1S203.JHJ0(V)
50
65
•45
I89.
5
40
64.
99
185
.6
"
55
67.07
203.
7
50
66.
02
194
•3
"
58*
. .
" +Na2S203 60
67.
4
2O6
•7
«
O
57
•63
136
Na2S203.2H20(V) 70
69.
06
223
.2
<«
10
59
•05
144.
2
70*
" +Na2S20,
20
61
.02
156.
5
40
67^4
206
•7
Na2S20,
25
62
•30
165-
3
50
67.
76
210
.2
"
30
63
•56
174.
4
60
68.
48
217
•3
«
35
65
.27
188
70
69.
05
223
.1
(i
27-5*
" +N02S203.H20 (V) 80
69-
86
231
.8
«
* tr. pt.
The authors adopted a new system of naming the hydrates, based upon their
mutual transition relations. These transitions occur in such a way that the
members of one group undergo transition into members of the same group and
not into members of another group. Those hydrates belonging to group (I) are
called primary hydrates, those belonging to group (II) are called secondary and
those belonging to the (III), (IV) and (V) groups are called tertiary, quaternary
and quintary respectively.
Commercial sodium thiosulfate is the primary pentahydrate, Na2S2O3.5H2O (I).
100 gms. alcohol dissolve 0.0025 gm. Na2S<jO3 and 0.0034 Sm- Na2S2O3.5H2O at
room temperature. (Bodtker, 1897.)
100 gms. alcohol of 0.941 Sp. Gr. dissolve 33.3 gms. sodium thiosulfate at 15.5°.
Data for the lowering of the freezing-point of Na2S2O3-5H2O by each of the fol-
lowing compounds: urea, glucose, cane sugar, NaCl, NaClO3, NaNO3 and Na2SO4
are given by Bautaric (1911).
SODIUM TUNGSTATE Na2WO4.2H2O.
SOLUBILITY IN WATER.
(Funk, igooa.)
-
Gms.
Na2W04 per
100 Gms.
Solution.
Mols.
Na2WO4
per
100 Mols.
H20.
Solid t o
Phase.
Gms.
Na2W04 per
100 Gms.
Solution.
Mols.
Na2WO4
100 Mols.
H20.
Solid
Phase.
-5
30.60
2.70
Na2WO4.ioH2O —3.
1 »)
41.67
4-37
Na3W04.2HjO
-4
3I-87
2.86
+ 0.
5
41-73
4-39
"
~~ 3
5 32-98
3-01
18
42 .O
4.40
M
— 2
34-52
3-23
21
42.27
4.48
"
0
3-52
43
.5
43 -98
4.81
"
+ 3
39-20
3-95
80
•5
47-65
5-57
II
5
41 .02
4.26
100
49-31
5-95
H
Sp. Gr. of sat. solution at 18° = 1-573-
solutions at 20°, see Pawlewski, 1900.
For Sp. Gr. determinations of aqueous
Fusion-point data for Na2WO4 + WO3 are given by Parravano (1909).
SODIUM URATE 676
SODIUM URATE C5H3N4O3.Na.
SOLUBILITY IN AQUEOUS SODIUM CHLORIDE AT 37°.
(d'Agostino, 1910.)
Gms. Mols; per Liter. Cms. Mols. per Liter. Gms. Mols. per Liter.
NaCl. 'c6H3N403.Na. ' NaCl. " C6H3N4O3Na. ' NaCl. " CsH3N4O3.Na.
O O.OO536 O.OIO84 O.002II O.O5II6 O.OOO5O
O.OO486 0.00340 0.01398 O.OOI72 0.06667 O.OOO34
0.00532 0.00321 0.02564 0.00102 0.07363 0.00032
O.O0865 O.OO256 O.040I2 0.00054 0.08595 O.00026
One liter of H2O dissolves 1 .5 gms. sodium urate at 37°. (Bechhold and Ziegler, 1910.)
One liter of serum dissolves 0.025 Sm- sodium urate at 37°.
SODIUM MetaVANADATE NaVO3.
SOLUBILITY IN WATER.
(MacAdam and Pierle, 1912.)
Solid Phase. f. *™ Solid Phase.
25 21.10 NaV03 2$ 15.3 NaVO3.2H2O
40 26.23 " 40 30.2
60 32.97 " 00 68.4
75 38.83 " 75 38.8 Navo,
Considerable time was required for attainment of equilibrium. The two solid
phases appear to exist for the whole rage of temperature and the conditions for
the transformation of one into the other were not ascertained.
SODIUM FluoZIRCONATE 5NaF.ZrF4.
IOO gms. H2O dissolve 0.387 gm. at 18°, and 1.67 gms. at IOO°. (Marignac, 1861.)
SPARTEINE C15H26N2.
SOLUBILITY IN WATER AND IN AQUEOUS SODIUM CARBONATE SOLUTIONS.
(Valeur, 1917.)
The author prepared solutions of recently distilled colorless sparteine (a =
— 2°46' in 5 cm. tube) in aqueous 5 per cent Na2CO3 and determined the tem-
perature at which clouding occurred in each.
t° of Gms. QsHasNu t° of Gms. Ci5H26N2 t° of Gms. CiBH26N,
Clouding. per 100 cc. Clouding. per 100 cc. Clouding. per 100 cc.
23-4 2.1 33.5 1.5 47 0.9
24 1-95 36.5 1-35 53 0.75
25 1.8 39.8 1.2 60.2 0.60
28.6 1.65 43.5 1.05 72.5 0.45
A saturated solution of sparteine in water was prepared, and after removing the
solid phase by centrif ugation, the amount of sparteine in the saturated solution was
determined with the aid of the data in the above table. Enough Na2CO3 and
H2O to yield 5 per cent Na2CO3 were added and the temperature of clouding ob-
served and compared with the above results. The average of these determina-
tions was 0.556 gm. sparteine per 100 cc. sat. solution in water at 10.8°.
SPARTEINE SULFATE Ci5H26N2.H2SO4.5H2O.
100 gms. H2O dissolve about 200 gms. sparteine sulfate at 15-20°.
100 cc. 90% alcohol dissolve about 20 gms. sparteine sulfate at 15-20°.
(Squire and Caines, 1905-)'
STEARIC ACID CH3(CH2)16COOH.
100 gms. H2O dissolve o.i gm. stearic acid at 37°.
100 gms. 5% aqueous solution of bile salts dissolve less than o.i gm. stearic acid.
100 gms. 5% aq. sol. of bile salt + i% lecithin dissolve 0.2 gm. stearic acid.
In the same solvents there is dissolved of sodium stearate, o.i, 0.2- and 0.7 gm.
respectively. (Moore, Wilson and Hutchinson, 1909.)
677 STEARIC ACID
SOLUBILITY OF STEARIC ACID IN AQUEOUS ETHYL ALCOHOL AT 25°.
(Seidell, 1910.)
Wt.% , f Cms. CnHjjCOOH Wt. % , . Cms. CnR^COOn
CzHjOH JPfa per 100 Cms. C2H6OH sS'Sl per 100 Cms.
in Solvent. Sat. Sol. in Solvent. Sat. Sol.
o 0.999 0.034 7° 0.865 0.80
20 0.967 0.04 80 0.841 1.63
40 0.932 o.io 90 0.818 3-3Q
50 0.911 0.18 95 0.807 5.55
60 0.888 0.40 loo 0.795 8.30
100 cc. f 94.3 Vol. % C2H6OH contain 0.0996 gm. CnHasCOOH at o° (do = 0.83 1 8) .
sat. sol.< 95.1 " " 0.1139 " " (^0 = 0.8287).
in [95.7 " " 0.1246 " " (do = 0.8265).
Saturation was approached from above without constant agitation. (Emerson, 1907.)
SOLUBILITY OF STEARIC ACID IN ETHYL ALCOHOL AT SEVERAL TEMPERATURES.
(Falciola, 1910.)
Cms. CnHjjjCOOH per 100 cc. of:
Absolute Alcohol. 75% Alcohol. 50% Alcohol.
10 0.9 0.15
20 2 ... 0.08(23°)
30 4-5 0.39 o.io
40 13.8 0-77 0.12
loo cc. sat; solution in 94.4 Vol. % CH3OH ("methylated alcohol" of d =
0.8183) contain 0.15 gm. CiyHasCOOH at +0.2°. Saturation was approached
from above without constant agitation. (Hehner and Mitchell, 1897.)
SOLUBILITY OF STEARIC ACID IN SEVERAL SOLVENTS AT 25°.
(Seidell, 1910.)
, f Cms. C17H35COOH
Solvent. d of Solvent. c^5 cli per 100 Cms.
Sat. Sol. Sat Sol
Acetone ^15= 0.797 0.815 4-73
Amyl Alcohol (iso) ^20=0.817 0.815 9.43
Amyl Acetate ^20=0. 875 0.867 11.19
Carbon Bisulfide ^25= 1.259 -1.163 19.20
Carbon Tetrachloride d25= 1.587 1-465 10.25
Chloroform d^= 1.476 1.332 15.54
Ether (abs.) ^22=0.711 0.744 20.04
Ethyl Acetate ^25=0.892 0.895 7-36
Nitrobenzene ^25=1.205 1.199 1.24
Toluene ^15=0.872 0.865 13.61
Fusion-point data for stearic acid + tristearin and for stearic acid -f- tri-
stearin + palmitic acid are given by Kremann and Kropsch (1914).
STILBENE C6H5CH:CH.C6H5.
Freezing-point data for mixtures of stilbene and p dimethoxystilbene are given
by Pascal and Normand (1913).
STRONTIUM ACETATE Sr(CH3COO)2.iH2O.
SOLUBILITY IN WATER.
(Osaka and Abe, 1911.)
t» Cms. Sr(CH3COO)2 s ,}d p,
* ' per 100 Cms. H2O.
0.05 36.93 Sr(CH3COO)2.4H20
25
40.19
5 39-91
35-03
38-82
10 43 .61
50
37-35
8 . 4 tr. pt. 43 . 1 " +Sr(CH3COO)2.*H20
70
36-24
8 43 . 5 Sr(CH3COO)2.*H20
80
36.10
10 42.95
90
36.24
15 41.00
97
36.36
Sr(CH3COO)2.JH20
STRONTIUM BENZOATE 678
STRONTIUM BENZOATE Sr(C7H6O2)2.H2O.
SOLUBILITY IN WATER.
(Pajetta, 1906.)
t°. 15-7°. 24.7°. 31.4°. 40.9°.
Gms. Sr(C7H602)2 per loo Gms. Solution 5.31 5.4 5.56 5.77
STRONTIUM BROMATE Sr(BrO3)2.
One liter of aqueous solution contains 0.9 gm. molecules or 309 gms. Sr(BrOj)j
at 1 8°. (Kohlrausch, 1897.)
STRONTIUM BROMIDE SrBr2.6H2O.
SOLUBILITY » IN WATER.
(Average curve from results of Kremers, 1858; and Etard, 1894.)
Gms. SrBr2 per 100 Gms. Gms. SrBr2 per 100 Gms.
Solution. Water. ' Solution. Water. '
o 46 85.2 40 55.2 123.2
10 48.3 93 50 57.6 135.8
20 50.6 102.4 60 60 150
25 51.7 107 80 64.5 181.8
30 52.8 111.9 I0° 69 222.5
Sp. Gr. of sat. solution at 20° approximately 1.70.
100 gms. abs. alcohol dissolve 64.5 gms. SrBr2 at o°. Sp. Gr. of solution = 1.21.
(Fonzes-Diacon, 1895.)
SOLUBILITY OF STRONTIUM BROMIDE IN AQUEOUS SOLUTIONS OF STRONTIUM
NITRATE AT 25°.
(Harkins and Pearce, 1916.)
Mols. per 1000 Gms. H2O.
" Sr(NO3)2. ' SrBr2.; '_]
o 4.3080
0.036 4-3I05
0.07216 4.3125
0.14568 4.3170
Gms. SrBr2
per 1000 Gms
I066. I
1066.95
1067.42.
1068.54
«¥cf
• Sat Sol.
1.7002
1.70325
1.72844
Mols. per 1000 Gms. H2O.
Gms. SrBr2
1068.8
1069. 17
1073-97
d^ot
Sat. Sol.
1.73766
I . 74866
1.77368
0
0,
I ,
30663
61124
,86lO
SrBr2.
4.3180
4.3190
4-3390
Data for equilibrium in the system strontium bromide, strontium oxide and
water at 25° are given by Milikau (1916).
STRONTIUM CAMPHORATE d C10H14O4Sr.4H2O.
SOLUBILITY IN AQUEOUS SOLUTIONS OF CAMPHORIC ACID AT 16-17°.
(Jungfleisch and Landrieu, 1914.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
C8H14(COOH)", C10H1404Sr. Sohd Phase. ^(COOH)", C10H14O4Sr. S«^ Phase.
1.25 I.4I3 C8H14(COOH)2 1.20 17.99
1.03 1.7705 (C10H1604)2Sr(C10H1,04)J O 16.95 CwH14O4Sr.4H2O
1.13 6.525 o 16.56
i. 20 12.452 o I2.86(atg8c) "
STRONTIUM CARBONATE SrCCX.
One liter of water dissolves 0.00082 gm. at 8.8° and 0.0109 Sm- at 24° by con-
ductivity method. (Holleman, 1893; Kohlrausch and Rose, 1893.)
One liter of water saturated with CO2 dissolves 1.19 gms. Sr(HCO3)2.
Data for the solubility of strontium carbonate in water containing CO2 at
pressures between 0.05 and i.i atmospheres are given by McCoy and Smith
(1911). The equilibrium constant is k = 1.29 X IO"2 with an average deviation
from the mean of 1.2 per cent. From this value, the solubility product is calcu-
lated to be Sr X CO8 = k3 = 1.567 X IQ-9.
679
STRONTIUM CARBONATE
SOLUBILITY OF STRONTIUM CARBONATE IN AQUEOUS AMMONIUM CHLORIDE.
(Cantoni and Goguelia, 1905.)
Cms. NH4C1 per
100 Cms. Solution.
Cms. SrCO3 per
1000 cc. Sat. Solution.
5-35 0.179
10 0.259
20 0.358
The mixtures were allowed to stand at 12-18° for 98 days.
Fusion-point data for SrCO3 + SrCl2 are given by Sackur (1911-12).
STRONTIUM CHLORATE Sr(ClO3)2.
100 gms. H2O dissolve 174.9 gms. Sr(ClO)2, or 100 gms. sat. solution contain
63.6 gms. at 18 . Sp. Gr. of solution is 1.839. (Mylius and Funk, 1897.)
STRONTIUM CHLORIDE SrCl2.6H2O.
SOLUBILITY IN WATER.
(Average curve from the results of Mulder; Etard; see also Tilden, 1884.)
Gms. SrCl2 per 100 Gms. Solid
to
Gms. SrCl2 per 100 Gms.
Solid
*
Solution.
Water.
Phase.
•
Solution. Water*
Phase.
— 20
26.O
35-1
SrCl2.6H2O
60
45-o
81.8
SrCl2.6H2O
O
30-3
43-5
M
70
46.2
85-9
SrCl2.2H20
10
32.3
47-7
"
80
47-5
90-5
M
2O
34-6
52-9
(I
100
50.2
100.8
M
25
35-8
55-8
"
I2O .
112. 8
M
30
37-o
58-7
"
140
55-6
125.2
M
40
39-5
65-3
"
160
58-5
141.0
u
50
42 .0
72.4
41
180
62.0
163.1
M
Transition temperature
about 62.5°.
Sp. Gr.
of sat.
solution at o°
= I-334J at
15° = 1.36.
SOLUBILITY OF STRONTIUM CHLORIDE IN AQUEOUS SOLUTIONS OF
HYDROCHLORIC ACID AT o°. (Engei, 1888.)
Mg. Mols. per TO cc. Solution.
*SrCl2.
S1.6
44-8
37-85
27.2
22. 0
14.0
4.25
HC1.
O
6.1
12.75
23-3
28.38
37-25
52-75
Sp. Gr. of
Solution.
•334
•304
.269
.220
.201
.167
i-'33
Grams per 100 cc. Solution.
SrCl2.
HCl.
40.9
0-0
35-5
2 .22
30.0
4-65
21 .56
8-49
17.44
10.35
II .09
I3-58
3-37
19.23
SOLUBILITY OF STRONTIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO-
BROMIC AND OF HYDROCHLORIC ACIDS AT 25°.
(Harkins and Paine, 1916.)
In Aqueous HBr. In Aqueous HCl.
Gms. Equiv. HBr j of
Gms. SrCl2
Gms. Equiv. HCl 4 of
Gms. SrClj
per looo Gms. T
H20. Sat. Sol.
per 100 Gms.
Sat. Sol.
per looo Gms. «
H2O. Sat. Sol.
per too Gms.
Sat. Sol.
o 1.4015
35-80
O.I55I 1.3953
35-17
0.06817 1.4020
35-47
0.5162 L3788
33-60
0.4191 I.4OIO
33-92
I.OI7 I-3563
31.42
0.9716 I-3992
3I-52
2.165 I-3065
26.33
I.I54 1-3995
20.78
9 . 205 i . 1498
3-055
STRONTIUM CHLORIDE
680
SOLUBILITY OF STRONTIUM CHLORIDE IN AQUEOUS SOLUTIONS OF ACIDS
AND OF SALTS AT 25°.
(Harkins and Paine, 1916.)
Aqueous g^ded gait ^%B °^
ution per 1000 Gms. Sat. Sol.
Gms. SrCl2
per loo Gms.
Sat. Sol.
Aqueous
Solution
of:
Gms. Equiv. , ,
added Salt *tt of
per looo Gms. Sat. Sol.
XlgvJ.
Gms.
er icx
SrCl,
3 Gms
CuCl2
o
7U4
i
.4200
34
•005
KNO3
0.09796
.4107
35
.86
"
a
276
i
•4595
30.40
0-4755
•4349
35
.90
HI
0
1641
z
.4058
34
.850
HNO3
0.1771
.4038
35
•52
tt
0
.4462
i
.4121
33
.28
"
0.3521
•4059
35
.40
ti
0
•7539
i
.4196
•52
tt
1.277
•4175
34
.04
KI
0.09199
i
•4093
35
•45
NaN03
0.3621
.4216
35
-63
"
o
5401
i
.4466
33
•79
"
0.5010
.4588
35
.60
"
o
6015
i
.4513
33
.60
"
3-553 1-5214
30
.88
"
I
445
i
.5154
30
.90
"
6.856 1-5581
25
•53
KC1
0
0719
i
•4032
35
.62
Sr(N03)2
0.1372 1.4113
35-42
"
o
433
i
.4085
34
.80
n
0.5766 1.4336
34
•47
a
0
8576
i
.4152
33
.89
tt
1.0988 1.4636
33
•30
tt
I
594
i
.4266
32
.40
"
3.318 1.6664
28
•97
Data for equilibrium in the system strontium chloride, strontium oxide and
water at o°, 25° and 40° are given by Milikau (1916).
100 gms. abs. methyl alcohol dissolve 63.3 gms. SrCl2.6H2O at 6°.
loo gms. abs. ethyl alcohol dissolve 3.8 gms. SrCl2.6H2O at 6°. (de Bruyn, 1892.)
SOLUBILITY OF STRONTIUM CHLORIDE IN AQUEOUS ETHYL ALCOHOL
SOLUTIONS AT 18°.
(Gerardin, 1865.)
Sp. Gr. of
Aq. Alcohol
ato°.
Wt.
per cent
Alcohol.
Gms. SrCl2
per 100 Gms.
Alcohol.
Sp. Gr. of
Aq. Alcohol
ato°.
Wt.
per cent
Alcohol.
Gms. SrClj
per 100 Gm
Alcohol.
0.990
6
49.8l
0-939
45
26.8
0.985
10
47-0
0.909
59
19.2
o-973
23
39-6
0-846
86
4-9
0.966
30
35-9
0.832
91
3-2
o-953
38
30-4
100 gms. 95% formic acid dissolve 23.8 gms. SrCl2 at 19°. (Aschan, 1913.)
100 cc. anhydrous hydrazine dissolve 8 gms. SrCl2 at room temp.
(Welsh and Broderson, 1915.)
Fusion-point data for SrCl2 + SrF2 are given by Plato (1907). Results for
SrCl2 + SrO and SrCl2 + SrSO4 by Sackur (1911-12). Results for SrCl2 + T1C1
by Korreng (1914) and results for SrCl2 + ZnCl2 by Sandonnini (i9i2a, 1914).
STRONTIUM CHROMATE SrCrO4.
SOLUBILITY IN WATER, ETC., AT 15°.
(Fresenius, 1891.)
Solvent.
Water
Aq. NH4C1 (5%)
Aq. CHaCOOH (i%)
Gms. SrCrO4
per loo
Gms. Solvent.
0.12
0.195
Gms. SrCrO4
Solvent. per 100
Gms. Solvent.
Aq. Ethyl Alcohol (29%) 0.0132
Aq. Ethyl Alcohol (53%) 0.002
68i
STRONTIUM CINNAMATE
STRONTIUM CINNAMATE (C6H6CH:CH.COO)2Sr.2H2O.
100 gms. H2O dissolve i gm. (C6H5CH:CH.COO)2Sr at I5°-2O°.
(Squire and Caines, 1905-)
100 gms. sat. aqueous solution contain 1.18 gm. (C«H6CH :CH.COO)2Sr at 15°
and 3.11 gms. at IOO°. (Tarugiand Checchi, 1901.)
STRONTIUM FORMATE Sr(HCOO)2.2H2O.
SOLUBILITY IN WATER. (Stanley, 1904.)
F.
0
ii
28.6
37-4
Si-4
Gms. Sr(HCOO)2
loo Gms. H2O.
7-02 (8.35)
8.08(9.54),
11.62 (13.25
13.01 (14.68
16.31 (17.83
per Solid Phase.
Sr(HCOO)2.2HiO
it
F.
67.5
86'
91.7
IOO
20.62 (21.76)
26.14 (26.36)
27-58 (27-57)
27.01 (27.07)
26.57 (26.72)
Sr(HCOO)2.2H2O
Sr(HCOO)2.H2O
There appears to be an error in the calculation of the results as given by the
author in his table. The figures given above in parentheses have, therefore,
been calculated from the weights of SrSC>4 recorded in the original table and
show the weight of Sr(HCOO)2 per 100 gms. of saturated solution.
STRONTIUM FLUORIDE SrF2.
One liter of water dissolves 0.1135 Sm- SrF2 at 0.26°, 0.1173 gm- at I7-4° an<3
0.1193 gm. at 27.4°, determined by the conductivity method. (Kohlrausch, 1908.)
STRONTIUM GLYCEROPHOSPHATE C3H7O2PO4Sr.2H2O.
100 gms. sat. solution in water contain 2.09 gms. anhydrous salt at 18° and 0.8
gm. at 60°. (Rogier and Fiore, 1913.)
STRONTIUM HYDROXIDE Sr(OH)2.8H2O.
SOLUBILITY IN WATER. (Scheibler, 1883.)
Grams per 100 Grams Solution. Grams per TOO cc. Solution.
V .
SrO.
Sr(OH)2.8H20.'
o
o-35
0.90
10
0.48
1.23
20
0.68
i-74
30
I .00
2-57
40
1.48
3.80
50
2.13
5 -46
60
3-03
7-77
70
4-35
ii . 16
80
6.56
16.83
90
12 .O
30.78
IOO
18.6
47 .71
SrO.
Sr(OH)2.8H2O.
o-35
0.90
0.48
1.23
0.68
1.74
1. 01
2-59
i-S1
3-87
2.18
5-59
3.12
8.00
4-55
11.67
7.02
18.01
13.64
34-99
22.85
58.61
MUTUAL SOLUBILITY OF STRONTIUM HYDROXIDE AND STRONTIUM NITRATE
IN WATER AT 25°. (Parsons and Perkins, 1910.)
j Gms. per 100 Gms. H2O.
,5}*°*, ' SrO as
Sat. Sol. Sr(OH)2.
Sr(NO.,)2.
1.481 o
79.27
1.492 0.38
79-47
1.494 0.78
80.83
1.506
.76
81.06
1.490
•71
74.27
1.419
.51
63-71
1.381
.41
56.30
1.327
.27
46.97
Gms. per 100 Gms. H2O.
Solid Phase.
Sr(OH)2.8H2O
ffcot '
at. Sol.
SrO as
Sr(OH)2.
sr(NOl>,.'
.267
I. II
37.81 Sr(OH)2.8H2O
.217
I.OI
28.80
.178
0.95
23-83
.148
0.91
17.96
.108
0.84
12.78
.079
0.81
8.96
•059
0-79
6. 29
1.033
0.78
4-45
STRONTIUM HYDROXIDE
682
SOLUBILITY OF STRONTIUM HYDROXIDE IN AQUEOUS SOLUTIONS AT 25°.
(Rothmund, 1910.)
Aqueous Solution of:
Mols.
Sr(OH)2.-
8H20
Cms.
Sr(OH)2
per
per Liter.
Liter.
Water alone
0.0835
10.16
0.5 n Methyl Alcohol
0.0820
9-97
" Ethyl Alcohol
0.0744
9-05
" Propyl Alcohol
" Amyl Alcohol
0.0708
8.61
(tertiary)
0.0630
7.66
" Acetone
0.0692
8.42
" Ether
0.0645
7-85
Aqueous Solution of:
0.5 n Glycol
" Glycerol
" Mannitol
Urea
" Ammonia
" Dimethylamine
" Pyridine
Mols.
Sr(OH)2.
8H20
per Liter.
O.O922
o. 1094
o. 1996
0.0820
0.0785
0.0586
o . 0694
Gms.
Sr(OH)2
tSu.
II. 21
24.29
9-97
9-55
8^44
Data for equilibrium in the system strontium hydroxide, phenol and water at
25° are given by van Meurs (1916).
STRONTIUM IODATE Sr(IO3)2.
100 gms. H2O dissolve 0.026 gm. at*i5°, and 0.72-0.91 gm. at 100°.
~ -Li
(Gay-Lussac; Rammelsberg, 1838.)
STRONTIUM IODIDE SrI2.6H2O.
SOLUBILITY IN WATER.
(Average curve from the results of Kremers, 1858; and Etard, 1874.)
Gms. SrI2 per
TOO Gms.
Solid
Solution.
Water.
' Phase.
0
62.3
I65-3
SrI2.6H20
20
64.0
177.8
"
40
65-7
I9I.5
««
60
68.5
217-5
"
80
73-o
270.4
•
t°.
Gms. Srls per
ioo Gms.
Solid
Solution.
Water. "
Phase.
90
78-5
365-2
SrI2.2H2O
100
79-3
383-I
"
120
80.7
4I8.I
it
I4O
82.5
47I-S
"
J75
85.6
594-4
<•
Transition temperature about 90°. Sp. Gr. of sat. solution at 20° = 2.15
ioo gms. sat. solution of strontium iodide in absolute alcohol contain 2.6 gms.
SrI2 at —20°, 3.1 gms. at +4°, 4-3 gms. at 39°, and 4.7 gms. at 82°. (Etard, 1874.)
Data for equilibrium in the system strontium iodide, strontium oxide and
water at 25° are given by Milikau (1916).
STRONTIUM PerlODIDE SrI4.
Data for the formation of strontium periodide in aqueous solution at 25°
are given by Herz and Bulla (1911). The experiments were made by adding
iodine to aqueous solutions of SrI2 and agitating with carbon tetrachloride.
From the iodine content of the CC14 layer the amount of iodine in the aqueous
layer can be calculated on the basis of the distribution ratio of iodine between
water and CCU. This furnishes the necessary data for calculating the amount
of the strontium periodide existing in the aqueous layer.
STRONTIUM IODOMERCURATE SrI2.HgI2.8H2O.
A saturated aqueous solution prepared by adding SrI2 and HgI2 in excess to
warm water and filtering when the temperature had fallen to 16.5° was found
to have the composition i.o SrI2.i.24 HgI2.i8.O9 H2O. The die. 5 was 2.5
(Duboin, 1906.)
683
STRONTIUM MALATE
STRONTIUM MALATE SrC4H4O5.
SOLUBILITY IN WATER.
(Cantoni and Basadonna, 1906.)
20
25
30
35
Gms. per 100
cc. Solution.
0.448
0-550
0.752
1.036
40
45
50
Gms. per 100
cc. Solution.
I-385
1-743
2.098
55
60
65
70
Gms. per 100
cc. Solution.
2.460
2.821
3.148
STRONTIUM MALONATE CH2(COO)2Sr.
SOLUBILITY IN WATER.
(Cantoni and Diotalevi, 1905.)
O
IO
20
Gms. per 100 cc.
Sat. Sol.
0-541
0.540
0.532
25
30
35
Gms. per 100 cc.
Sat. Sol.
O.52I
0.499
0.478
40
45
50
Gms. per too cc.
Sat. Sol.
0.464
0-453
0-443
STRONTIUM MOLYBDATE SrMoO4.
100 gms. H2O dissolve 0.0104 gm. SrMoO4 at 17°.
STRONTIUM NITRATE Sr(NO3)2.
SOLUBILITY IN WATER.
(Berkeley and Appleby, 1911.)
(Smith and Bradbury, 1891.)
t°.
dtoi
Sat. Sol.
G
Sr(N(
loo Gr
53)2 pe
ns. H2
3.
t°.
dtoi
Sat. Sol.
Gms. c i'j
Sr(N03)2per pSh°^
100 Gms. H2O. Phase-
0.58
.28561
40.
124
Sr(NO3)2.4H2O
30-74
.51282
90.086 Sr(NO,)1
14.71
.39380
00.
867
"
47-73
•5II50
91.446
26.40
.48831
82.
052
«
61.34
. 51048
93.856 "
29.06
.51098
87.
648
«
68.96
•51057
95.576
29.3*
" +Sr(N03)2
78.98
.51091
97.865 ««
30.28
.51441
88 !
577
Sr(NOj)2
88.94
•5II74
100. 136 "
32.58
.51408
88.
943
"
The determinations were made with very great accuracy.
SOLUBILITY OF STRONTIUM NITRATE IN AQUEOUS ALCOHOL AT 25°.
(D'Ans and Siegler, 1913.)
Wt. %
CAOH
Solvent
Gms. per 100 Gms.
m Sat. Sol.
Solid Phase.
Wt. %
C2HBOHiE
Solvent.
Gms
i
. per 100 Gms.
Sat. Sol. •
Solid Phase.
• QzHsOH.
Sr(N03)2.
C2H5OH.
Sr(NO3)2.
0
0
44
•25
Sr(NO3)2.4H2O
IO
6
40.
05
Sr(NOj)2 (unstable)
4
i-7
42
.8
"
15
05
9
5
36,
>j
" (unstable)
6
2.6
42
.1
«
18
.8*
12
35
34
3
" +Sr(N03)2.4H20
10.8
4-95
40
•4
"
20
6
13
.8
33
2
SrCNOdi
16
7-95
37
.6
"
40
65
32
35
20.
5
"
20*
12.35
34
•3
" +Sr(N03)J
59
9
53
6
IO,
5
«
O
o
46
.6
Sr(NOa)2 (unstable)
79
,2
77
15
2,
6
«
6
3-45
42
• 7
" "
99
4
99
38
0,
02
«
* Tr. pt.
100 cc. anhydrous hydrazine dissolve 5 gms. Sr(NOa)2 at room temp.
(Welsh and Broderson, 1915.)
STRONTIUM NITRITE Sr(NO2)2.H2O.
100 cc. sat. solution in water contain 62.83 gms. Sr(NO2)2.H2O at 19.5°.
41 90% alcohol " 0.42 " " " 20°.
" abs. alcohol " 0.04 " " " 20°.
(Vogel, 1903.)
STRONTIUM NITRITE 684
SOLUBILITY OF STRONTIUM NITRITE IN WATER.
(Oswald, 1912, 1914.)
Gms. Sr(NO2)s Gms.
t° per 100 Gms. Solid Phase. t°. per 100 Gins? Solid Phase.
Sat. Sol. Sat. Sol.
— 1.3 II-3 Ice 35 43-1 Sr(NQd,.HiO
- 3-1 J9-6 " 52.5 46.5
- 7-7 35-5 60.5 49.3
-6.8 32.8 " +Sr(N02)2.H20 65.5 50.7
- 2.3 33.4 SrCNO^.HjO 82.5 54
- 0.3 34-5 92 56.6
+ 19 39-3* 98 58.1
* d = 1.4461.
STRONTIUM OXALATE SrC2O4.H2O.
One liter of water dissolves 0.0328 gm. SrC2O4 at 1.35°, 0.0444 gm. at 15.9°,
0.0461 gm. at 18°, 0.0575 gm- at 3l-7° and 0.0617 Sm- at 37.3°, determined by
the conductivity method. (Kohkausch, 1908.)
One liter of sat. aqueous solution contains 0.057 gm- SrC2O4 at o°, 0.077 gm.
at 20° and 0.093 Sm- at 4°°- (Cantoni and Diotalevi, 1905.)
SOLUBILITY OF STRONTIUM OXALATE IN AQUEOUS ACETIC ACID SOLUTIONS
AT 26°-27°.
(Herz and Muhs, 1903.)
Normality of
Acetic Acid.
Gms. per 100 cc. Solution.
Normality ol
Acetic Acid.
Gms. per 100 cc. Solution.
CH3COOH.
SrC204.H2O. '
CH3COOH.
SrCA.H20
O
0
O.OO9
3.86
23.16
0.0598
0.58
3.48
0.0526
5-79
34-74
o . 0496
1-45
8.70
0.0622
16.26
O.OO6O
2.89
17-34
0.0642
STRONTIUM OXIDE SrO.
Fused SrCl2 dissolves 18.3 gms. SrO per 100 gms. of the fused melt at 910°.
(Arndt., 1907.)
STRONTIUM PERMANGANATE Sr(MnO4)2.
100 gms. of the sat. solution in water contain about 2.5 gms. Sr(MnO4)2 at o°.
(Patterson, 1906.)
STRONTIUM SALICYLATE (C6H4OH.COO)2Sr.2H2O.
100 gms. sat. solution in water contain 3.04 gms. (C6H4OHCOO)2Sr at 15° and
20.44 gmS. at IOO°. (Tarugi and Checchi, 1901.)
SOLUBILITY OF STRONTIUM SALICYLATE IN AQUEOUS ALCOHOL AT 25°.
(Seidell, 1909, 1910.)
Wt. %
2H,OH in
Solvent.
d^ol
Sat! Sol
Gms. (C6H4.OH.-
COO)2Sr.2H2O
per 100 Gms.
Sat. Sol.
Wt. %f
CaHsOH in
Solvent.
Sat. Sol.
Gms. (C6ILOH-
COO)2Sr.2H20
per 100 Gms.
Sat. Sol.
0
I.O22
5-04
60
0.923
7-15
10
1. 006
4.88
70
0.893
5-90
20
0-993
5-22
80
0.859
4.40
30
0.982
6.20
90
0.824
2.56
40
0.966
7.70
92.3
0.815
2.02
50
0.948
8.08
100
0.790
0.44
The solid phase was (C6H4OH.COO)2Sr.2H2O in all cases except the solution
m 100 per cent alcohol, in which partial dehydration and conversion of the
crystalline salt to an amorphous bulky white powder occurred.
Gms. QHASr
Gms. C.H.O
t°.
per 100 cc.
t°.
per zoo cc,
Sat. Sol.
Sat. Sol.
0
0.052
2O
0.270
5
0.076
25
0.382
10
O.III
30
0.451
15
0.177
35
0.413
685 STRONTIUM SUCCINATE
STRONTIUM SUCCINATE C4H4O4Sr.
100 gms. sat. solution in water contain 0.439 gm. C4H4O4Sr at 15° and 0.215
gm. at IOO°. (Tarugi and Checchi, 1901.)
SOLUBILITY OF STRONTIUM SUCCINATE IN WATER.
(Cantoni and Diotalevi, 1905.)
Gms. C^x^OjSr
t°. per 100 cc.
Sat. Sol.
40 0.375
45 0.389
50 0.424
STRONTIUM SULFATE SrSO4.
One liter of water dissolves 0.1133 gm. SrSO4 at 2.85°, 0.1143 gm. at 17.4°
and o. 1 143 gm. at 32.3°, determined by the conductivity method. (Kohlrausch, 1908.)
SOLUBILITY OF STRONTIUM SULFATE IN AQUEOUS SOLUTIONS OF AMMONIUM
ACETATE AT 25°.
(Marden, 1916.)
Gms. per too Gms. Sat. Sol. Gms. per too Gms. Sat. Sol.
CHsCOONH*. SrS04. CHaCOONH,. SrSO4. "
0 0.0151 10.68 0.0942
2.13 0.0451 21.37 O.II5
5.34 0.0732
SOLUBILITY OF STRONTIUM SULFATE IN AQUEOUS CALCIUM NITRATE AT
ROOM TEMPERATURE
(Raffo and Rossi, 1915.)
Analyzed solutions of Sr(NO3)2, Ca(NO3)2 and CaSO4 were mixed at 60° and
allowed to stand at room temperature I to 2 days. The resulting SrSO4 was
determined and the difference between the amount found and the amount
which would have resulted if all the Sr(NO3)2 had been converted to SrSO4f
was taken as the amount of SrSO4 dissolved. Gradually increasing concentra-
tions of Ca(NO3)2 were used.
Gms. per 100 cc. Sat. Sol. Gms. per 100 cc. Sat. Sol.
"Ca(NOdj. SrS04. ' 'Ca(NOa)2. SrSO4. "
0.5 0.0483 4 0.1489
1 0.0619 5 0.1698
2 0.1081 6 0.1955
3 0.1275
SOLUBILITY OF STRONTIUM SULFATE IN AQUEOUS SOLUTIONS OF
HYDROCHLORIC, NITRIC, CHLORACETIC AND FORMIC ACIDS.
(Banthisch, 1884.)
ec. of Aq.
Acid con-
taining i
Mg. Equr
ineachcasi
In Aq. HC1
Gms. per zoo cc.
In Aq. HNOs
Gms. per 100 cc.
Sol.
In Aq.CH2ClCOOH
Gms. per 100 cc. Sol.
In Aq. HCOOH
Gms. per 100 cc.
^ol.
CH2C1
COOH.
SrS04.
I'. ' HC1.
SrSO4.
HN03.
SrSO4.
HCOOH,
. SrSO4.
0.2
18.23
0
.161
31
•52
0
.381
. . .
o-5
7.29
0
.207
12
.61
0
•307
. . .
...
x.o
3-65
0
.188
6
•3o
0
.217
94-47
O.O26
46.02
0.024
2 -O
1.82
0
.126
3
•!5
0
.138
47-23
O.O22
. . .
...
IO.O
0.36
0
.048
0
•63
0
.049
ioo gms. 95 per cent formic acid dissolve 0.02 gm. SrSO4 at 18.5°. (Aschan, 1913)-
STRONTIUM SULFATE 686
SOLUBILITY OF STRONTIUM SULFATE IN AQUEOUS SODIUM CARBONATE AT 25°.
(Herz, rgio.)
Freshly prepared and dried SrSO4 was shaken 5 days with aqueous sodium
carbonate solutions and the supernatant clear solutions analyzed.
Normality of Aqueous Gm. Mols. per Liter Sat. Sol.
M, CQ /Na*COA t NaaCO,. Na2SO4'
V 2 / 2 2
0.6025 0.0382 0.5643
I.2O5 0.076 I.I29
2-41 0-153 2.257
SOLUBILITY OF STRONTIUM SULFATE IN SULFURIC ACID SOLUTIONS.
f. Conc.ofH2SO, GmSGS^0ASd.100 Authority.
ord. concentrated 5 . 68 . (Sturve, 1870.)
fuming 9.77 "
" 91% O.o8 (Varenne and Paulean, 1881.)
70 Sp. Gr. 1.843 = 99% 14 (Garside, 1875-)
ord. Absolute H2S04 21.7* (Bergius, 1910.)
* per 100 cc. Sat. Sol.
SOLUBILITY OF STRONTIUM SULFATE IN AQUEOUS SALT SOLUTIONS.
(Virck, 1862.)
In Aq. NaCl. In Aq. KC1. In Aq. MgCl2. In Aq. CaCl2.
' (a.) (6.) (a.) (6.) (a.) (6.) ' (a.) (ft.) " '
8.44 0.165 8.22 0.193 1.59 0.199 8-67 0.176
15.54 0.219 12.54 0.193 4.03 0.206 16.51 0.185
22.17 0.181 18.08 0.251 13.63 0.242 33.70 0.171
(a) = Cms. salt per 100 gms. aq. solution. (6) = Cms. SrSO4 per 100 gms.
solvent.
STRONTIUM TARTRATE SrC4H4O6.3H2O.
SOLUBILITY IN WATER.
, (Cantoni and Zachoder, 1905.)
Gms. Gms. Gms.
t°. SrC4H4O6.3H2p per t°. SrC^O^H-sO per t° SrC.HA^HaO per
100 cc. Solution. too cc. Solution. 100 cc. Solution.
O O.II2 25 0.224 60 0.486
10 0.149 3° 0.252 70 0.580
15 0.174 40 0.328 80 0.688
20 0.200 50 0.407 85 0.755
SOLUBILITY OF STRONTIUM TARTRATE IN AQUEOUS SOLUTIONS OF ACETIC ACID
AT 26°-27°.
(Herz and Muhs, 1903.)
Normality of Gms. per ico cc. Solution. Normality of Gms. per too cc. Solution.
Acetic Acid. CH3COOH. SrC4H4O6.3H20. Acetic Acid. CH3COOH. ' SrC4H4O6.3H2O.
o o 0.227 3-77 21.85 1.051
o-5<55 3-39 0.678 5.65 33.90 0.982
1.425 8.15 0.864 16.89 101.34 0.184
2.85 17.10 0.996
STRONTIUM (Di) TUNGSTATE SrW2O7.3H2O.
100 cc. H2O dissolve 0.35 gm. at 15°. (Lefort, 1878.)
687
STRYCHNINE
STRYCHNINE
SOLUBILITY IN SEVERAL SOLVENTS.
Gms. CnH-aNjOj
Gms. QiH^N
Solvent.
t°.
per 100 Gms. Solvent.
t-.
per zoo Gms
Solvent.
Solvent.
Water
ord.t.
0.014 C1
Carbon Tetrachloride
20
0.158 (5)
u
20
0.0125(2
« Cf
20
0.22 9)
"
20
0.0143(3
(t 11
T7
0.645 IC
(C
25
0.016 (4) Chloroform
25
10.25 6]
(f
20
0.021 (5)
25
16.6 i/
Aq. io%NHs
2O
°-°33 (3) Diethylamine
20
1-7 (3)
Aq. 3% H3BO3 in 50%
Glycerol ord. t.
3-5 i
Ethyl Acetate
Ether
20
20
0.197 (s
0.043 (5
C2H6OH (^=0.83)
15-20
0.71 7
M
25
0.018 (4
" (^=0.83)
2O
0-833 3
" sat. with H2O
2O
0-051 (5
" (<*=o.83)
25
v *f
0.91 (4
Glycerol
15
0.25
" +10%
NHs 20
0.256 (3) Petroleum Ether
2O
0.0093(5]
" (^=0.785)
25
0.70 (6
Piperidine
20
0.7 (3)
CH3OH (^=0.796)
25
0.49 (6
Pyridine
20
i.S (3)
Aniline
20
20 (3
«
26
1.24 (i:
Amyl Alcohol
25
/
0-55 (4
Aq. 50 % Pyridine
20-25 2.43 (8)
Benzene
2O
0.77 (s
Water sat. with Ether
20
0.017 (S>
M
25
0.76 (6
Oil of Sesame
20
0.061 (2]
(i) Baroni and Barlinetto (1911); (2) Zalai (1910); (3) Scholtz (1912); (4) U. S. P. 8th ed.; (5) Mullet
[1903); (6) Schaefer (1913); (7) Squire and Caines (1905); (8) Dehn (1917); (9) Gori (1913); (10)
Holty (1905).
lindelmeiser (1901); (u)
SOLUBILITY OF STRYCHNINE IN AQUEOUS ALCOHOL AT i5°-2oa.
(Squire and Caines, 1905.)
Per cent Alcohol in Solvent 20 45 60 70
Cms. C2iH22N2O2 per 100 cc. solvent 0.024 0.125 0.25 0.40
90
0-59
SOLUBILITY OF STRYCHNINE IN MIXTURES OF ETHER AND CHLOROFORM AT 25°.
(Harden and Dover, 1916.)
Per cent
CHC13 in
Mixed Solvent.
100
90
80
70
60
Cms. CziH-sNzOz
per 100 Gms.
Mixed Solvent.
15-3
2.77
i-5
0.65
Per cent
CHC13 in
Mixed Solvent.
Gms. QiHaNjOj
per 100 Gms.
Mixed Solvent.
50
0-35
30
0.21
20
0-15
10
0.09
O
O.O2
SOLUBILITY OF STRYCHNINE IN MIXED SOLVENTS AT 25°.
(Schaefer, 1913.)
Gm-
One volume of C2H5OH+4 vols. CHCla
One volume of C2H5OH+4 vols. CeH6
One volume of CH3OH +4 vols. CHCla
One volume of CH3OH +4 vols. C6H6
per
25
5
25
6. 7
DISTRIBUTION OF STRYCHNINE BETWEEN WATER AND CHLOROFORM AT 25°.
(Seidell, igioa.)
Gm. CK
per 15 cc
Added
4-iS cc.
Gms. C21H22N2O2 Recovered per 15 cc:
0.00$
0.025
0.12$
O.62C
H2O Layer (a).
O.0006
O.OOIO
O.OO2I
0.0099
CHC13 Layer (b).
O.OI03(?)
0.0253
0.1299
0.6225
(6)
25.2
61
64
STRYCHNINE 688
STRYCHNINE ARSENATE C21H22N2O2.H3AsO44H2O(.iiH2O).
loo gms. sat. solution in water contain 4.53 gms. C2iH22N2O2.H3AsO4 at 25°.
(Puckner and Warren, 1910.)
IOO gms. CHCU dissolve 0.085 gm. C2iH22N2O2.H3AsO4 at 15°. (Hill, 1910.)
STRYCHNINE FORMATE C2iH22N2O2.HCOOH.2H2O.
SOLUBILITY IN WATER AND IN ALCOHOL.
(Hampshire and Pratt, 1913.)
Solubility in Water. Solubility in Abs. Alcohol.
t«, Gms. Salt per ^.o Gms. Salt per
loo Gms. H2O. loo Gms. C2H6OH.
19-5 30-59 18.5 10
24 39-68 20 10.3
27 44-25 22 10.64
STRYCHNINE HYDROBROMIDE CnHEN-A.HBr.
IOO CC. H2O dissolve 1.54 gms. of the salt at I5°-2O°. (Squire and Caines, 1905.)
loo cc. 90% alcohol dissolve 1.04 gm. of the salt at I5°-2O°.
STRYCHNINE HYDROCHLORIDE
IOO cc. H2O dissolve 2.86 gms. of the salt at I5°-2O°. (Squire and Caines, 1905.)
loo cc. 90% alcohol dissolve 1.37 gms. of the salt at I5°-2O°.
100 gms. CHCls dissolve 0.592 gm. of the salt at 15°. (Hill, 1910.
STRYCHNINE NITRATE
SOLUBILITY IN SEVERAL SOLVENTS.
Gms. Salt Solvent. Gms. Salt
Solvent. t°. per 100 cc. t°. per 100 cc.
Solvent. Solvent.
Water 15 1.4 (i) CHaOH 25 0.345 (3
15-20 1.6 (2) CHCU 25 1.25 (3
25 2.38(4) i vol. CJfcOH+4 vols. CHO. 25 5 (3
80 12.5 (4) i vol. C2HfiOH+4 vols. C6H6 25 0.66 (3
9o%C2H6OH 15-20 0.83
i5 0.77
b. pt. 3.45
2) i vol. CHaOH+4 vols. CHCU 25 4 (3
i) i vol. CHaOH+4 vols. C6H6 25 i (3
i) Glycerol 25 1.66 (4)
100% CzHfiOH 2*5 0.37 (3)
(i) Dottdgio); (2) Squire and Caines (1905); (3) Schaefer (1913); (4) U. S. P. VIII ed.
DISTRIBUTION OF STRYCHNINE NITRATE BETWEEN WATER AND CHLOROFORM
AT 25°.
(Seidell, igioa.)
Gms. CzjH-aNzOis.HNOa Gms. Q^zjNzOz.HNOs per 15 cc.: a
Added per 15 cc. t • *• \ -•
HjO + 15 cc-CHCla. H2O Layer (a). CHC13 Layer (b).
0.005 0.0051 o.oo3o(?)
0.025 0.0222 0.0042 5.3
0.125 O.IOI7 0.0243 4-2
0.625 0.3250 0.1698 2
STRYCHNINE OXALATE
loo gms. H2O dissolve 1.13 gms. of the anhydrous salt at about 15°.
(Dott, 1910.)
STRYCHNINE PERCHLORATE C21H22N2O2.HC1O4.
100 gms. HaO dissolve 0.022 gm. perchlorate at 15°.
(Hofmann, Roth, Hobold and Metzler, 1910.)
689
STRYCHNINE SULFATE
STRYCHNINE SULFATE
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent.
Water
«
90% C2H6OH
94% "
94% "
100% "
CHaOH
t°.
15-20
25
80
15-20
25
60
25
25
Gms. Salt
per ioo cc.
Solvent.
2.08 (i)
3-23 (2)
16.6 (2]
0.74 (i)
1.9 (')
6.2 2
0.8 3
8-33 3
Solvent.
CHCU
i vol. C2H50H+4vols. CHCU
i vol. C2H50H+4 vols. CeHe
i vol. CHsOH+4 vols. CHCls
i vol. CHaOH+4 vols.
Glycerol
15
25
25
25
25
25
25
15
Gms. Salt
per ioo cc.
Solvent.
0.05
0.31
0-43
12.8
0.725 (3)
25 (3)
12.5
18
(4)
8
8
(3)
I
(i) Squire and Caines (1905); (2) U. S. P. VIII; (3) Schaefer (1913); (4) Hill (1910).
d Tartrate.
/ Tartrate.
Racemic Tartrate,
14.14
9.48
14.02
17.72
11.50
19.12
22.9
I4-52
24.70
15.60
17.02
35-18
22.90
38.42
STRYCHNINE TARTRATE
SOLUBILITY OF d, I AND OF RACEMIC STRYCHNINE TARTRATE IN WATER.
(Dutilh, 1912.)
Gms. of Each Separately per 1000 gms. H2O. ,.
t°. d Tarti
7-35
16
25
27
30
40
SOLUBILITY OF MIXTURES OF d AND / TARTRATES AND OF RACEMIC STRYCHNINE
TARTRATE IN WATER.
(Ladenburg and Doctor, 1899.)
Results for d + / Tartrate. Results for Racemic Tartrate.
Gms. Anhydrous Gms. Anhydrous.
t°. Salt per ioo Gms. Solid Phase. t°. Salt per ioo Gms. Solid Phase.
H20. H20.
7 1.48 S°%d+S%l 7 1-39 Racemic Tartrate
19 i-95 *9 i-90
27 2.38 27 2.33
35 3-02 35 3-i7
42 3-75 42 3-92
ioo gms. sat. solution in water contain 0.45 gm. anhydrous strychnine acid
tartrate at about 15°. (Dott, 1910.)
SUBERIC ACID C6H12(COOH)2.
SOLUBILITY IN WATER.
(Lamouroux, 1899.)
t°. o°. 15°. 20°. 35°.
Gms. CeHi2(COOH)2 per ioo cc. sol. 0.08 0.13 0.16 0.45
50°.
0.98
65°.
2.22
SOLUBILITY OF SUBERIC ACID IN ALCOHOLS AT 4°.
(Timofeiew, 1894.)
Gms. C6Hi2(COOH)2 per ioo Gms.
Alcohol.
Sat. Sol. Alcohol.
Methyl Alcohol 20.32 3 2 . 04
Ethyl Alcohol 15.5 1 8 . 44
Propyl Alcohol 12.2 13.9
ioo gms. 95 per cent formic acid dissolve 2.13 gms. C6Hi2(COOH)2 at 19.5°.
(Aschan, 1913.)
Data for the distribution of suberic acid between water and ether at 25° are
given by Chandler, 1908.
SUCCINIC ACID
SUCCINIC ACID (CH2)2(COOH)2.
690
SOLUBILITY IN WATER.
(Miczynski, 1886; van der Stadt, 1902; Lamouroux, 1899; for other concordant results, see Bourgoin,
1874; Henry, 1884.)
*°- Gms. (CH2)2(COOH)2 per too
Gms. Succinic
Anhydride
(CH2)2COCOO
per too Gms.
Mol.
Per cent.
Gms. H2O.
cc. Solution.
H20.
(CH2)2COCOO:
H2O.
0
2.80
2.78(L.)
2-34
99.58
0.42
IO
4.51
4
3-80
99-32
0.68
20
6.89
5-8
5-77
98.97
1.03
25
8.06
7
6.74
98.80
1.20
30
10.58
8-5
8.79
98.44
1.56
40
16.21
12.5
13-42
97.64
2.36
50
24.42
18
19-95
96.53
3-47
60
35.83
24-5
28.77
95-07
4-93
70
51.07
40. ii
93.26
6.74
80
70.79
54.08
91.12
8.88
89.4
95-4.'
70.62
88.71
ii. 29
104.8
146.3
IOI.2
84.57
15-43
II5.I
188.5
126.8
81.4
18.6
134-2
335-4
187.8
74-72
' 25.28
159-5
748.2
295.2
65.27
34-73
180.6
1839
. . .
408.5
57-6
42.4
182.8
00
542-3
5°
50
174.4
. . .
. . .
808.5
40.7
59-3
153.3
. . .
2239
19.86
80.14
128
. . .
8865.
5-89
94.11
II8.8-II9
00
0
100
The following very careful determinations of the solubility of succinic acid
in water are given by Marshall and Bain (1910).
t°. o°. 12.5°. 25°. 37. S°- 50°- 62.5°. 75°.
Gms. (CH2)2 (COOH)2
per 100 gms. H2O 2.75 4.92 8.35 14 23.83 39.35 60.37
SOLUBILITY OF SUCCINIC ACID IN AQUEOUS SOLUTIONS OF SALTS AND OF
ACIDS AT 25°.
(Herz, igiob, 1911.)
In Aq. HBr.
Gms. per Liter.
In Aq. HC1,
Gms. per Liter.
In Aq. KBr.
Gms. per Liter.
In Aq. KC1.
Gms. per Liter.
HBr.
C4H604.
HC1. C4H6O4.
KBr. C4H6O4.
KC1.
C4H604.
0
8l.2I
18.45 66.
25
0
81.
21
28.34
75.58
79-
3
57-38
45-6 50,
,78
65-
45 75-
58
77.56
74-39
274-
4
32.83
87-9 35
,42
260.
5 69.
68
150.7
69.68
166.6 27
•75
502.
i 62.
59
267
61.41
In Aq.
KI.
In Aq. LiCl.
In
Aq. NaCl.
Gms. per Liter.
Gms. per Liter.
Gms
. per Liter.
Solid
KI.
C4HeO4.
LiCl.
C4He04-
' NaCl.
C4H604.
Phase.
0
8l.2I
0
81.
21
l8.7
74-39
C4Hfl04
46,
,48
79-12
7.63
70.
86
32.73
69.68
"
102
9
77-93
23.32
62.
59
64.3
61.41
H
, ' ,
57-66
47-
24
I32.I
49-55
"
ny
29.
Si
289.4
27.16
"
176.4
20.
07
3I5-I
22.44
NaCl
231-5
14.
318
4-72
"
691
SUCCINIC ACID
SOLUBILITY OF SUCCINIC ACID IN AQUEOUS SOLUTIONS OF POTASSIUM
SUCCINATE AND VlCE VERSA AT SEVERAL TEMPERATURES.
(Marshall and Cameron. 1907.)
Gms. per 100 Gms
4o. Sat. Sol.
Solid Phase.
Gms. per 100 Gms.
t°. Sat. Sol.
Solid Phase.
H2C4H404.
K2C4H4O4. H2C4H4O4.
K2C4H404.
0
2
•71
o
H2C4HA •
25
7-88
0
H2C4H404
0
7
,26
8.
09
" +KH3(C4HA)2
25
9-
965
3-
17
"
o
7
.86
7-
66
" "
25
12.
77
8.
4
"
0
8
.24
9-
95
KH3(C4HA)2
25
17-
6
14-
15
cc
0
8,
. ii
12.
77
"
25
18.
i
14-
3
" +KH,(CJH,04),
0
7-87
15-
47
" +KHC4H4O4.2H2O
25
15-
36
18.
48
KH3(C4H404)2
0
0
40.
2
K2C4H404.3H20
25
7
23-
6
" H-KHC^O*
14
i
.468
41.
3
K2C4H404+KHC4H4O4
25
13-
06
23-
81
KHC4H4O4
+KHC4H4O4.2H20
25
ii.
98
24.
43
"
15.
9 i
-7
34-
36
KHC4H404.2H2O+KHC4H4O4
25
9-97
25
"
20
6
•39
o
H2C4H4O4
25
6.
61
28.
6
"
20
7
.48
i.
85
"
25
2.
6
38.
2
"
20
14
•63
ii.
64
"
25
2.
ii
40.
6
CC
20
15
•03
13-
32
" +KH3(C4H404)2
25
I,
<>3
48.
7
" +K2C4H404.3H20
20
13
•32
18.
46
KHsCC^O^z
25
0.
13
56.
IS
K2C4H404.3H20
20
12
-74
22.
45
" +KHC4H404
25
O
58.
05
"
20
II
-7
22.
91
KHC4H4O4
40
12,
9
0
H2C4H404
20
I
42.
I '
"
40
25
• 5
16.
83
" +KH3(C4H4O4)2
20
I
•05
47-
3
" +K2C4H404.3H20
40
19
25-
481
^- H-3^ 04^X404) 2"i K. XI (^4X14^
20
O
•985
48.
i
K2C4H404.3H20
40
*5
•83
26.56
KHC4H4O4
20
0
.909
48.
75
"
40
o
62.
10
KjC^C^HjO
20
o
-159
54-
3
"
20
0
56.6
SOLUBILITY OF SUCCINIC ACID IN ALCOHOLS AND IN ETHER.
(Timofeiew, 1891, 1894; at 15°, Bourgoin, 1878.)
Solvent.
Abs. Methyl Alcohol
Abs. Ethyl
90% "
Abs. Propyl
Abs. Ether
Isobutyl Alcohol
Gms. (CH2)2(COOH)2 per 100 Gms. Solvent at:
10.51
5.06
2. II
+15°.
12.59
7-51
1.265
+21-5°.
19.40
9-49
4-79
2-73
+39°-
28.7
15
7-53
loo gms. 95 per cent formic acid dissolve 2.06 gms. (CH2)2(COOH)2 at 18.5°.
(Aschan, 1915.)
DISTRIBUTION OF SUCCINIC ACID BETWEEN WATER AND AMYL ALCOHOL
AT 20°.
(Herz and Fischer, 1904.)
Millimols JC4H«O4
per 10 cc.
Gms. C4H«O4
per 100 cc.
Millimols iC4H«O4
per 10 cc.
Gms. C4HgO4
per 100 cc.
Alcohol
Layer.
0.1888
0.3643
0.7077
1.440
2.715
Aq.
Layer.
0.2684
0.5252
1-0373
2.1266
4.0495
Alcohol
Layer.
o. 1114
0.215
0.418
0.850
1.603
Aq.
Layer.
0.1584
0.310
0.612
1.255
2.391
Alcohol
Layer.
3.899
5-199
6-334
7.119
Aq.
Layer.
6.0795
8.099
10. 170
11.555
Alcohol
Layer.
2.302
3.069
3-739
4.202
Aq.
Layer.
3-588
4-779
6
6.821
SUCCINIC ACID
692
SOLUBILITY OF SUCCINIC ACID IN AQUEOUS ACETONE AT 20°.
(Herz and Knoch, 1904.)
cc. Acetone per
zooicc. Solution.
O
10
20
30
40
50
C4HgO4 per 100 cc. Solution.
Millimols.
107.8
127.4
155-8
186.7
225-4
254-3
Gms.
6.363
7.5I9
9.194
II. O2
I3.30
15.01
cc. Acetone per
100 cc. Solution.
C4H6O4 per zoo cc. Solution
Millimols. Gms.
60
275.7 16.27
70
278.5 16.44
80
265.3 15-66
90
201.9 11.91
iOO
5L5 3-04
SOLUBILITY OF SUCCINIC ACID IN AQUEOUS GLYCEROL SOLUTIONS AT 25°.
(Herz and Knoch, 1905.)
Wt. %
Glycerol in
Solvent.
C4H6O4 per 100 cc.
Solution.
Sp. Gr. of
Solutions.
Wt. %
Glycerol in
Solvent.
C4H«
iO4 per zoo cc.
solution.
Sp. Gr. of
Solutions.
Millimols.
Gms.
Millimols.
Gms.
0
133
•4
7.874
I
.0213
40.95
105.
8
6.244
I. I I 20
7-
15
128
.2
7.566
I
.0407
48.70
99.
9
5.896
1.1298
20.
44
118
•3
6.982
I
.0644
69.20
88.
5
5.223
I . 1804
31-
55
109
•7
6.476
I
.0897
IOO*
74-
6
4.440
1.2530
* Sp. Gr. of Glycerol = 1.2555. Impurity about 1.5 per cent.
DISTRIBUTION OF SUCCINIC ACID BETWEEN WATER AND ETHER AT
AND 25.5°.
(Pinnow, 1915.)
Results at 15
Gm. Mok. per Liter.
0
c
c
6.
6.
6.
Results at 20
Gm. Mols. per Liter.
0
c
c'
6.
6.
6.
6.
Results at 25.
Gm. Mols. per Liter.
c
7-
7-
7-
52
52
7i
Aqueous
Layer (c).
0.474
0.2585
O.II75
Ether
Layer (c*).
0.0783
0.0415
0.0187
05
23
28
Aqueous
Layer (c).
0.644
0.312
O.I5I
0.0405
Ether
Layer (c')-
0.096
0.046
0.0218
O.OO6
71
87
93
75
Aqueous
Layer (c).
0.3293
0.1768
0.0894
Ether "
Layer (c').
0.0438
0.0235
0.0116
Very careful determinations of this distribution at o° and at 25°, in which the
ionization of the succinic acid in the two solvents is taken into consideration, are
given by Chandler, 1908. Two determinations at o° and two at 15° are quoted
by Kolossovsky, 1911. Earlier data for this system are given by Nernst, " Theo-
retical Chemistry," 3rd English edition, p. 496.
BromSUCCINIC ACID CHBr(CH2)(COOH)2 (m. pt. 159°).
SOLUBILITY IN ALCOHOLS AT 22°.
(Timofeiew, 1894.)
Gms. CHBr(CH2)(COOH)2 per 100 Gms.
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Sat. Solution.
56-5
45-5
33-1
Alcohol.
129.7
83.6
49.4
Data for the distribution of monobromsuccinic acid between water and ether
at 25° and for dibromsuccinic acid between water and ether at 25° are given by
Chandler (1908).
Data for the melting-points of mixtures of the following pairs of optical anti-
podes are given by Centnerszwer (1899).
d + / Chlorsuccinic Acid.
d 4- i Chlorsuccinic Acid.
d Chlorsuccinic Acid + I Bromsuccinic Acid.
i Chlorsuccinic Acid + 1 Bromsuccinic Acid.
d + / Benzylaminosuccinic Acid.
d -f- / Aminosuccinic Acid.
693
SUCCINIMIDE
SUCCINIMIDE
CO
SOLUBILITY IN WATER AND IN ETHYL ALCOHOL.
Interpolated from original results.
In Water.
(Speyers, 1902.)
In Ethyl Alcohol.
Wt.of
Mols. per
Cms. per
Wt.of
Mols. per
Gms. per
t°. I CC.
100 Mols.
100 Gms.
I CC.
ioo Mols.
ioo Gms
Solution.
H20.
H20.
Solution.
QHfiOH.
QH6OH
o 1.025
1.58
8.69
0.815
0.88
1.89
10 1.035
2.4
14
0.809
i-35
2.7
20
.052
4
23
0.8o6
2
4.1
25
.067
5-9
33
0.805
2-5
5-3
30
.086
8
45
0.804
3-i
6.8
4P
.I2O
12.8
70
0.809
4.9
10.5
50
•145
17.8
96
0.816
7.8
16
60
.167
22.6
124
0.835
12.3
26.5
70
.189
27.5
152
0.873
80
.204
32-8
0-954
Freezing-point data (solubilities, see footnote, p. i), are given for ethylsuc-
cinimide + bromotoluene and for ethylsuccinimide + p xylene by Paterno and
Ampola (1897).
SUCCINIC NITRILE (Ethylene Cyanide) CNCH2CH2CN.
The solubility of succinic nitrile in water and also in aqueous sodium chloride
solutions at various temperatures has been determined by Schreinemakers (1897),
and the results presented in terms of mols. of nitrile per ioo mols. of nitrile -j- H2O.
The following calculations of these results to gram quantities was made by
Rothmund. (Landolt and Bernstein's, " Tabellen " 1906.)
t°.
18.5
20
39
45
Gms. CNCH2CH2CN per ioo Gms.
Gms. CNCH2CH2CN per ioo Gms.
Aq. Layer.
IO.2
II
22
Nitrile Layer.
92
91-5
85.2
Aq. Layer.
53-5 33-2
55 40-3
55.4 crit. temp.
Nitrile Layer.
66.4
62.8
Very complete data for the system succinic acid nitrile, ethyl alcohol and
water, determined by the synthetic sealed-tube method, are given by Schreine-
makers (i8o.8c). Results for the system succinic acid nitrile, cane sugar and
water are given by Timmermans (1907).
SUGAR Ci2H22Ou (Cane Sugar.)
SOLUBILITY IN WATER.
(Herzfeld, 1892; see also Courtonne, 1877.)
per
ioo Gms.
O
5
10
15
20
25
30
35
Solution.
Water.
64.18
179.2
64-87
184.7
65.58
190.5
66.33
197
67.09
203.9
67.89
2II.4
68.70
219.5
69.55
228.4
40
45
70
80
90
ioo
Gms. CigHaOu per
ioo Gms.
Solution.
Water.
70.42
238.1
71.32
248.7
72.25
260.4
74.18
287.3
76.22
320.4
78.36
362.1
80. 61
415.7
82.97
487.2
Sp. Gr. of sat. solution at 15° = 1.329; at 25° = 1.340.
ioo gms. H2O dissolve 212 gms. cane sugar at 25°, determined by means of
Pulf rich's refractometer. (Osaka, 1903-08.)
SUGAR
694
SOLUBILITY OF SUGAR IN AQUEOUS SALT SOLUTIONS AT 30°, 50°, AND 70°.
Interpolated from original results.
(Schukow, 1900.)
Gms.
per 100 grams EfeO in Aq. Solution of:
loo Gms. H2O. KC1.
KBr.
KN03.
Nad.
CaCl2.
3?
0
219.5
219.5
219.5
219.5
219.5
10
216
218
217
2IO
197
tt
20
221
22O
216
211
189
"
30
228
224
216
219
I92
M
40
237
228
217
233
20O
K
50
218
25O
218
M
60
269
243
50
0
260.4
260.4
260.4
260.4
260.4
(i
10
26l
262
260
255
239
(I
20
266
266
261
260
228
«
30
274
272
262
269
228
U
40
284
276
262
284
236
"
50
296
280
263
302
253
(<
60
276
70
0
320.5
320.5
320.5
320.5
320.
(C
10
326
324
321
323
295
u
20
334
328
324
330
286
u
30
345
334
327
344
286
n
40
357
34i
33i
361
295
u
50
37°
349
• 334
384
308
u
00
384
357
337
406
327
SOLUBILITY OF CANE SUGAR IN SATURATED AQUEOUS SALT SOLUTIONS AT
31.25°. (Kohler, 1897.)
Salt.
CH3COOK
C3H7COOK
C3H4.OH.(COOK)3
.K2C08
KC1
CH3COONa
NaCl
Gms. Sugar per 100 Gms.
Solution.
49.19
56.0
62.28
59-93
62.17
Water.
324.8
306.1
265.4
246.5
237.6
236.3
Gms. Sugar per 100 Cms-
Solution.
Na2C03 64-73
KNO3 61.36
K2S04 66.74
CH3COOCa 60.12
Na2SO4 52.20
CaCl2 42-84
MgS04 46-52
Water.
229.2
224.7
219.0
190.0
I83-7
I35-I
119.6
SOLUBILITY OF CANE SUGAR IN AQUEOUS ALCOHOL SOLUTIONS AT 14°.
(Schrefeld, 1894.)
Wt.
per cent
AlcohoL
Wt.
per cent
Sugar.
Gms. Sugar per 100
CC. Alcohol-H2O
Mixture.
Wt.
per cent
Alcohol.
Wt.
per cent
Sugar.
Gms. Sugar per 100
cc. Alcohol-HsO
Mixture.
0
66.2
I95.8
50
38.55
62.7
5
64.25
179.7
60
26.70
36.4
10
62.20
164.5
70
12.25
13-9
20
58.55
141 .2
80
4.05
4-2
30
54-05
II7.8
90
o-95
0-9
40
47-75
91 .
IOO
c-oo
O-O
695
SUGAR
SOLUBILITY OF CANE SUGAR IN AQUEOUS ALCOHOL SOLUTIONS.
(Scheibler, 1872; correction, 1891.)
Results at o°.
Results at 14°.
Results
at 40°.
Per cent
Sp. Gr. of
Cms. Sugar Sp. Gr. of
Cms.
per 100 cc. Solution.
Gms. Sugar
Alcohol
Solution a,t
per 100 cc. Solution at
A
per 100 cc.
by Vol.
17.5°.
Solution. 17-5°.
Sugar.
C2H5OH.
H20.
Solution.
O
1-325
85.8 1.326
87.5
0
45-iQ
IO
1.299
80.7
• 300
8l-5
3-91
44.82
95-4
20
1.236
74.2
.266
74-5
8.52
43-83
90
30
1.229
65-5
•233
67.9
13-74
41.87
82.2
40
1.182
56.7
.185
58
20. 24
40.38
74-9
50
1. 129
45-9
•131
47-1
28.13
38.02
63-4
60
1.050
32.9
.058
33-9
37-64
34-47
49-9
70
0.972
18.2 0.975
18.8
46.28
29-57
3i-4
80
0.893
6.4 0.895
6.6
6I.I5
21.95
13-3
90
0.837
0.7 0.838
0.9
7I.I8
12.83
2-3
97-4
0.806
0.08 0.808
0.36
77-39
3-28
0-5
100 gms. absolute methyl alcohol dissolve 1.18 gms. cane sugar at 19°.
(de Bruyn, 1892.)
SOLUBILITY OF CANE SUGAR IN
AQUEOUS ACETONE AT 25°.
(Herz and Knoch, 1904.)
Sp. Gr. of
cc. Acetone
Gms. Sugar
Gms. per 100 cc.
Solution.
Solutions.
Solvent.
Solution.
H20.
(CH3)2CO
CiuHaOn
1.3306
0
89.8
43-3
0
89.8
1.2796
20
76.7
42.9
8.4
76.7
1.2491
30
72.1
39-5
13-4
72.1
1.2002
40
59-3
39-8
20.9
59-3
I. 1613
45
52.5
39
24.6
52-5
Above 45 cc. acetone per 100 cc. solvent the solution begins to separate into
two layers. The lower of these contains 51 gms. sugar per 100 cc. and has Sp.
Gr. 1.1522. The upper layer contains so little sugar that the amount could not
be determined by the method employed. 100 cc. evaporated in a vacuum desic-
cator left a residue of 3.68 gms. Above the concentration of 80 cc. acetone per
100 cc. solvent the two layers unite. In pure acetone 100 cc. solution gave a
residue of 0.18 gm. sugar.
Sugar.
Cane Sugar (Sucrose)
Milk Sugar (Lactose)
Grape Sugar (Glucose)
Fruit Sugar (Fructose)
Galactose
Maltose
Mannose
Raffinose
SOLUBILITY OF SEVERAL SUGARS IN PYRIDINE AT 26°.
(Holty, 1905.)
Gms. Sugar
Formula.
d C6H12O6.H20
CeHxA
C18H32016.5H20
J26 of Sat. Sol.
per 100 Gms.
Sat. Sol.
6-45
0.981
2.18
1.005
7.62
1.052
18.49+
1.0065
5-45(?)
98.10*
. . .
29.9*
75*
(Dehn, 1917.)
* It is uncertain whether these figures refer to gms. per 100 gms. sat. solution or gms. per 100 gms.
pyridine at 2o°-2S°.
100 gms. aq. 50 per cent pyridine dissolve the following gms. of sugars at 20°-
25°; sucrose, 38.5; maltose, 43.07; mannose, 78.70; lactose, 1.98; fructose,
85.42; galactose, 68.3; glucose, 49.17; raffinose, 8.76. (Dehn, 1917.)
100 gms. trichlorethylene dissolve 0.004 gm. cane sugar at I5°- (Wester & Bruins, 1914.)
For additional data on Galactose, see p. 305 and on Glucose, see p. 306.
SUGARS
696
SOLUBILITY OF MILK SUGAR (LACTOSE) HYDRATE AND ft ANHYDRIDE IN
WATER.
(Hudson, 1904, 1908.)
It was found that the saturation point was reached very slowly with this
compound. From the results, it was concluded that "aqueous solutions of
milk-sugar contain two substances in equilibrium and that the mutarotation of
milk-sugar results from the slow establishment, in cold solutions, of the equi-
librium of the balanced reaction, Ci2H24Oi2 (Hydrate) <=± H2O + Ci2H22Ou (ft-an-
hydride).
The final solubility of hydrated milk sugar was determined by approaching
saturation from below and from above with mixtures of water and excess of once
recrystallized hydrated milk sugar. These were constantly rotated until equilib-
rium was reached (one week was allowed in all cases). The filtered saturated
solutions were evaporated to dryness and the crystalline residues, consisting of
the a and ft anhydrides, weighed.
o
15
25
39
Cms. CuHsAi
per 100 Gms.
Sat. Sol.
10.6
14-5
17.8
24
t-.
49
64
74
89
Gms.
per 100 Gms.
Sat. Sol.
29.8
39-7
46.3
58.2
The initial solubility, obtained by agitating an excess of milk sugar hydrate
with water for a few minutes, was somewhat less than one-half the above figures,
at temperatures up to 25°.
The final solubility of ft anhydrous milk sugar was difficult of determination
on account of the high concentration and instability of the saturated solution
below 92°. At o° the final saturation was hastened by addition of o.i n NHaOH
solution. At o°, 42.9 gms. Ci2H22On per 100 gms. sat. solution were found and
at 1 00°, 61.2 gms.
SOLUBILITY OF SEVERAL SUGARS IN AQUEOUS ALCOHOL AT 20°.
(Hudson and Yanovsky, 1917.)
Sugar.
a. Arabinose
ft Cellose
ft Fructose
ft «
ft "
a Galactose
a "
ft, a Glucoheptose
a Glucose
a.
a " hydrate
ft Glucose
a Lactose hydrate
a Lyxose
ft Maltose hydrate
ft Mannose
ft
ft Mellibose Dihydrate
a Rhamnose Hydrate
a. "
a Xylose
Sucrose
Trehalose Dihydrate
Raffinose Pentahydrate
Gms. Anhydrous Sugar
Formula.
Solvent.
per 100 cc.
Solution.
Initial
Final
Solubility.
Solubility.
CSHM05
80% C2H5OH
0.74
1.94
CpHaOu
20% «
3-2
4-7
C.H^O,
80% "
13-4
27.4
it
95% "
1.8
4-2
"
Methyl Alcohol
5-2
ii. i
QHtfOg
60% C2H6OH
i.i
3- r
"
80% "
0.27
0.65
C7Hi4O7
20% "
4
4-5
C,H1204
80% "
2
4-5
Methyl Alcohol
0.85
1.6
C6H1206.H20
80% C2H6OH
I-3
3
C,H1206.
80% "
4-9
9.1
CaByOuJB^O
4o%
i.i
2.4
C5HU05
QO% "
5-4
7-9
CaHaOu.HiO
60% "
3
4-75
80% "
2.4
13
"
Methyl Alcohol
0.78
4-4
Ci2H22O4.2H2O
80% C2H5OH
0.76
j.j
C6HU06.H20
100% «
8.6
9-5
"
70% "
8.2
9.6
CBH1005
80% "
2.7
6.2
CaHaOu
80% "
3-7
3-7
CuHaOu.aHtO
70% "
1.8
1.8
CigHszOjg.sHzO
50% "
1.4
1-4
697 SUGARS
SOLUBILITY OF SORBOSE AND GULOSE IN WATER AND ALCOHOLS.
(de Bruyn and van Ekenstcin, 1900.)
Gms. Sugar per 100 cc. Sat. Sol. in:
Sugar. M.-pt.
H,O at 100°. CH3OH at 17°. QHBOH at 17°.
d Sorbose 151 0.22 1.70 1.02
/ Sorbose 150 0.23 1.68 i
/ Gulose 150 0.24 1.72 1.04
100 gms. H2O dissolve 108 gms. maltose at 2O°-25°. (Dehn, 1917.)
100 gms. H2O dissolve 14.3 gms. raffinose at 2O°-25°. "
SOLUBILITY OF PHENYLHYDRAZONES AND /3 NAPHTHYLHYDRAZONES OF THE
SUGARS IN WATER AND IN ALCOHOLS AT i6°-i8°.
(van Ekenstein and de Bruyn, 1896.)
The hydrazones were prepared by adding to a concentrated and warm solution
of the sugar the equivalent quantity of the hydrazine dissolved in the molecular
quantity of glacial acetic acid. The precipitated hydrazones were recrystallized
from 30 to 50 per cent alcohol. No details in regard to the method of obtaining
saturation or of analysis of the solutions are given.
Gms. Compound per too cc. Sat. Sol. in:
Phenylhydrazone of: M.-pt.
Water. CH3OH. QH5OH.
Methyl Mannose 178 0.2-0.06 0.59 0.05-0.02
Arabinose 161
" Rhamnose 124 " very si. sol. "
" Galactose 180
Ethyl Galactose 169 ... ... o. i
Mannose 159 ... ... 0.2
" Arabinose 153 ... ... 0.4
" Rhamnose 123 ... very si. sol.
Amyl Galactose 116 ... ... 0.6
' Mannose 134 ... 3.5
' Arabinose 120 ... 3.6
Rhamnose 99 ... very si. sol. 6.5
Glucose 128 ... ... 1.2
' Lactose 123 ... ... 0.4
Allyl Galactose 157 ... ... 0.3
" Mannose 142 ... 0.7
" Arabinose 145 ... 0.5
Rhamnose 135 ... ... ...
Glucose 155
Lactose 132 ... ... 0.2
" Melibose 192 ... ... 0.3
Benzyl Galactose 154 ... 0.9 0.08
" Mannose 165 ... °-5S 0-2
Arabinose 170 ... 0.4 0.06
Rhamnose 121 ... 15.4 6.7
Glucose 150 ... 0.5 o.io
" Lactose 128 ... 0.9 0.06
/3 Naphthyl Galactose 167 0.14 ... 0.24*
Mannose 157 0.18 ... 0.25*
Arabinose 141 0.22 ... 0.62*
Rhamnose 170 0.20 ... 0.44*
Glucose 95 0.25 ... 5*
Xylose 70 0.32 ... 6.62*
Lactose 203 0.07 ... 0.2*
Maltose 176 ... ... 0.4*
Melibose 135 ... ... 1.3*
* Solvent 96 per cent CjHjOH.
SUGARS
698
SOLUBILITY OF THE BENZALIC COMPOUNDS OF SOME POLYATOMIC ALCOHOLS
AT I6°-I8°.
(de Bruyn and van Ekenstein, 1899.)
No details of the determinations are given,
sufficiently exact for use in identifying hexites.
Name of Compound.
Dibenzalerythritol
Monobenzalarabitol
Dibenzaladonitol
Dibenzalxylitol
Dibenzalrhamnitol
Monobenzal-d-Sorbitol
Dibenzal-d-Sorbitol
Tribenzalmanni tol
Tribenzal-Mditol*
Tribenzal-d-talitolt
Dibenzaldulcitol
Dibenzalperseitol
M.-pt.
2OI (Fischer)
152
175
203
175
I63
213-8
215-8
2IO
215-20
230-5
(Meunier)
(Fischer)
It is stated that the results are
Gms. Compd. Dissolved per 100 cc.
Sat. Sol. in:
Acetone.
Chloroform.
Alcohol.
0-34
3.64
0.02
0.64
1*36
O.I4
I. 10
0.85
0.70
.2-55
I. 10
very
easily soluble
5-44
o. 16
O.IO
0.42
8-75
0.10
0.47
0.17
O.O5
0.30
4.42
trace
0.42
0.83
trace
0.04
trace
O.02
* Prepared from / idonic acid. t Prepared from d talonic acid.
ioo gms. sat. solution in pyridine contain 0.47 gm. mannitol at 26°. (Holty, 1905.)
100 gms. sat. solution in pyridine_contain 2.5(?) gms. erythritol at 26°.
SULFANILIC ACID NH2.C6H4.S03H.H2O.
SOLUBILITY IN WATER.
(Philip, 1913; results for 60° and over by Dolinski, 1905.)
Solid Phase.
NH2.C6H4.SO3H.2H2O
NH2.C6H4.S03H.H2O
Gms. NH2.-
C6H4.S03H
t .
per ioo Gms.
Sat. Sol.
0
0.444
7.2
0.622
13-3
0.841
18.9
1.093
18.9
I.I37
25-1
1.384
31-1
1.662
37-2
2.0O4
Gms. NH2.-
4°.
C6H4.S03H
per ioo Gms,
Solid Phase.
Sat. Sol.
44
2.44
NH2.C6H4.S03H.H20
44
2.36
NH2.C6H4.SO3H
47-5
2.52
"
54-5
2.85
u
60
3.01
"
70
3.65
"
80
4-32
"
IOO
6.26
"
SULFONIUM PERCHLORATES
SOLUBILITY IN WATER.
(Hofmann, Hobold and Quoos, 1911-12.)
Name.
Formula.
Trimethyl
Ethyl dimethyl
Propyl "
n Butyl "
Ethylene dismeihyl
Vinyl dimethyl
Trimethylene dismethyl
Sulfine Perchlorate (CH3)3sciO4
C2H5(CH3)2SC104
C3H7(CH3)2SC104
C4H9(CH3)2SC1O4
C2H4(C2H6SC104)2
C2H3.S(CH3)2.C104
Per ioo Gms. H2O.
'
Gm. Mols.
= Gms.
16.5
0.0784
13.84
15-9
o. 1191
22.31
15
0.0590
12.04
15
0.0607
13.24
18
0.0423
14.86
18
0.0731
13.75
18
0.0402
14.68
699 SULFONIUM IODIDE
TriethylSULFONIUM IODIDE S(C8H6),I.
IOO gms. H2O dissolve 431 gms. S(C2H5)3l at 25°. (Peddle and Turner, 1913.)
IOO gms. CHC13 dissolve 47.7 gms. S(C2H6)3l at 25°. (Peddle and Turner, 1913.)
SULFUR S.
In a series of papers by Aten (1905-06, 1912, 1912-13, 1913, 1914 and I9i4a),
the preparation and properties of the four known modifications of sulfur are de-
scribed. These are designated by the symbols, S\, S^, ST and Sp.
S\ is ordinary rhombic sulfur and its molecule is considered to be composed of
eight atoms of sulfur, Ss.
SM is the insoluble, so-called amorphous sulfur.
S^ is obtained when ordinary sulfur is heated above its melting-point and
quickly cooled; it is especially easily prepared by warming S\ in sulfur chloride.
Its molecule is probably represented by 84.
Sp was discovered by Engel and is prepared by mixing concentrated HC1,
cooled to o°, with saturated sodium thiosulfate solution. The precipitated
NaCl is removed by filtration and the solution extracted with toluene. The
aqueous layer soon yields a cloudy precipitate of Sp. The molecule of this
sulfur is considered to have the composition S6.
SOLUBILITY OF SULFUR (S\) IN SULFUR MONOCHLORIDE (SaCk) DETERMINED
BY THE MELTING-POINT METHOD.
(Aten, 1905-06.)
t° of Melting. M "* Solid Phase. t° of Melting. ' ™ Solid Phase.
Mixure
— 1 6 4.3 Rhombic S 83.5 67 Rhombic S
06" 95.6 8l.8
+ 17.9 9-9 " 86 8l.8 MonoclinicS
36.8 I7.I 103.2 88.4
55.2 28.5 110.4 95
65.6 40.3 118.8 loo
77-7 55-4
SOLUBILITY OF SULFUR (S,-) IN SULFUR MONOCHLORIDE (S2C12)
(Aten, 1912-13.)
A preliminary experiment showed that if a solution of Sx in sulfur monochlo-
ride, saturated at 20°, is heated to 170° and cooled, it will then dissolve as much
Sx as already required to saturate it. The following determinations were made
by sealing known amounts of Sx and S2C12 in tubes, heating them to 100° for
several hours and then cooling quickly to the indicated temperatures and shak-
ing for \ hour in the case of the o° and 25° results and 2 hours in the case of the
— 60° results. The saturated solutions were analyzed by oxidizing with HC1
+ HNO3 + Br and titrating the H2SC>4, after removing the volatile acids.
Atoms S per 100 Atoms S+S2C12 in: Atoms S per 100 Atoms S+SjClj in:
Original Saturated Solution at: Original Saturated Solution at;
Mixture. ^60°. o°. +25°. ' Mixture. -60°. o°. +25°.
o ii. 6 36.1 53.5 79-4 65.2 72
10 18.1 40.1 57.6 80. i 66.1 71.6
28.7 31.9 47.4 62 89.9 ... ... 82.1
49.9 42.9 56 66.4 90.1 80.5
60. i 47.7 59.9 69.4 94.6 87.7
69-1 ... 72.8 98 93.4
Results similar to the above are also given (Aten, 1912), for mixtures previ-
ously heated to 50°, 75° and 125°. All the data confirm the formation of the
the new modification S*-.
SULFUR 700
SOLUBILITY OF SULFUR (S*-) IN SULFUR MONOCHLORIDE (S2C12) AT 25°.
(Aten, 1912, 1913.)
The samples were heated to the temperatures indicated and rapidly cooled
and powdered. The method of determining the solubilities is not described.
Atoms S Dis-
Previous Treatment of Sample. solved per 100
Atoms S+S2C12.
Unheated Sulfur 53 . 5
Mixture of Rhombic and Amorphous
Sulfur 54-5
Rhombic Sulfur heated tO 125° 56-58 . 5 (depending on excess of S present.)
" " " " 165° 60 (determined immediately.)
" " " " 165° 59.5 " after i hr.)
" 165° 57.5 " " 24hrs.)
" 165° 53.2 " 8 days.)
SOLUBILITY OF SULFUR (ST) IN TOLUENE AT o° AND AT 25°.
(Aten, 1913.)
Comp. of Mix- Solubility in Atom % S. Comp. of Mix- Solubility in Atom % S.
ture in Atom » . ture in Atom / • *
Per cent S. At o . At 25 . per cent S. At o . At 25 .
35 2.88 5.94 74 4.05 7.52
47 6.65 77 3.90
54 3.26 6.76 80 4.22
57 3-30 6.88 83 ... 7.93
73 7-45 85 8.08
These results show that the greater the excess of Sv, the greater the solubility.
It was found that under the same conditions, unchanged rhombic sulfur gives
constant figures irrespective of the excess of S present. At o°, 2.59 atom per cent
S\ was found and at 25°, 5.65 atom per cent.
SOLUBILITY OF SULFUR (SM) IN CARBON DISULFIDE AND CARBON
TETRACHLORIDE.
(Wigand, 1910.)
When "insoluble" sulfur (SM) is treated with CS2 or CCU, a small amount
dissolves, depending upon the length of time of contact, temperature and nature
of the solvent but not on the relative amount of solvent. This action is ex-
plained on the assumption that a partial transformation of SM to soluble sulfur
S\, takes place.
Data for the fusion points of mixtures of rhombic sulfur and "insoluble"
sulfur (Sj,) and for monoclinic sulfur and "insoluble" sulfur (S/J are given by
Kruyt (1908).
SOLUBILITY OF SULFUR IN LIQUID AMMONIA.
(Ruff and Hecht, 1911.)
At the temperatures o° to 40°, the solutions were constantly shaken for 3 to 4
days. For the results at the lower temperatures the solutions were saturated
at room temperature then cooled, partially evaporated and shaken 4 to 6 hours.
The saturated solutions were analyzed by evaporation of the ammonia by means
of a current of hydrogen, absorbing in HCl and converting to the platinic chloride
for weighing. The S residues were dried at 100°, with proper precautions, and
weighed.
*o Gms. S per 100 Gms. f0 Gms. S per 100 Cms.
Sat. Solution. Sat. Solution.
-78 38.6* +I6.4 25.65
-20.5 38.1* 30 21
o 32.34 40 18.5
* This figure corresponds to the compound S(NH3)3 = 38.5% S.
yoi SULFUR
SOLUBILITY OF SULFUR IN AQUEOUS SODIUM SULFIDE SOLUTIONS.
(Kuster and Heberlein, 1905.)
The results are expressed in terms of x which represents the number of S
atoms dissolved for each Na2 in the solution. The figures, therefore, show the
atomic ratio of S to Naa in the saturated solution and at the same time, the sulfur
content of the compound NaaSx which is formed. In order to find the actual
amount of sulfur dissolved per liter, it is only necessary to multiply the x value
by the normality of the aqueous sodium sulfide solution used as solvent in the
particular case.
A series of determinations made at 25°, by agitating aqueous sodium sulfide
solutions with crystalline sulfur until equilibrium was reached, and then diluting
each solution with an equal volume of water and shaking with excess of sulfur
until equilibrium was again reached, gave the following results:
Normality of the Aq. * in the Result- Normality of the Aq. x in the Result-
NazS Solution. ing NaaS». NauS Solution. ing NajS-j.
4 4-475 0.125 (32hrs.) 5.225
2 (2 hrs.) 4.666 0.0625 5. 239
i 4.845 0-03125 5.198
0.5 4.984 0.015625 5.034
0.25 5.115 0.007812 (128 hrs.) 4-456
The figures in parentheses in the above table show the number of hours re-
quired for attainment of equilibrium in these three cases. The authors also
made determinations of the influence of temperature on the amount of sulfur
dissolved, and found that for a normal Na2S solution, the x value did not vary
appreciably from the figure given above, over the range o° to 50°.
Results are also given showing the influence of the presence of NaCl and of
KOH on the amount of sulfur dissolved by aqueous Na2S solutions. In the
former case the solubility was distinctly lowered, while in the latter it was notably
increased.
SOLUBILITY OF SULFUR IN:
Tin Tetrachloride. Amyl Alcohol.
(Gerardin, 1865.) (Gerardin.)
••• ~SJ- as. -• -Xar
99 5.8 SolidS 95 1.5 Solid S
101 6.2 " IIO 2.1-2.2 "
no 8.7-9.1 " 112 2.6-2.7 Liquids
112 9.4-9.9 Liquids 120 3.0
121 17.0 " 131 5.3 "
SOLUBILITY OF SULFUR IN AQUEOUS ACETONE AT 25°.
(Herz and Knoch, 1905.)
Wt. Per cent Sulfur per 100 cc. Solution. Sp. Gr. of
in SoKent. Millimols. Cms. ' Solution.
ioo 65 2.084 0.7854
95.36 45 1.442 0.7911
90.62 33 1.058 0.8165
85.38 25.3 o.8n 0.8295
SULFUR 702
SOLUBILITY OF SULFUR IN ETHYL AND METHYL ALCOHOLS.
Cms.
t*. Alcohol. per 100 Gms. Authority.
Alcohol.
15 Abs. Ethyl 0.051 (Pohi.)
18.5 O . 053 (de Bruyn — Z. physik. Chem. 10, 781, 'pa.)
b. pt. O .42 (Payen — Compt. rend. 34, 356, '52.)
18.5 Abs. Methyl O.O28 (de Bruyn.)
SOLUBILITY OF SULFUR IN BENZENE AND IN ETHYLENE DIBROMIDE.
(Etard, 1894; see also Cossa, 1868.)
In C6He. In C2H4Br2.
Gms. S Gms. S Gms. S Gms. S
t°. per loo Gms. t°. per 100 Gms. t°. per 100 Gms. t°. per 100 Gms.
Solution. Solution. Solution. Solution.
o i -o 70 8.0 o 1.2 50 6.4
10 1.3 80 10.5 10 1.7 60 8.4
20 1-7 QO 13.8 20 2.3 70 II.4
25 2.1 100 17.5 25 2.8 80 16.5
30 2,4 no 23.0 30 3.3 90 24.0
40 3.2 120 29.0 40 4.4 100 36.5
50 4-3 130 36-o
60 6.0
RECIPROCAL SOLUBILITY OF SULFUR AND BENZENE, DETERMINED BY THE
SYNTHETIC METHOD.
(Kruyt, 1908-09.)
Wt. % S in Limiting t° of ^Homogeneity. \yt. % S in Limiting t° of ^Homogeneity.
Mixture. Lower. Upper. Mixture. ' Lower. Upper. "
41.5 146 247 79.8 141 230
55.2 158 230 81.4 138 above 246
74.5 157 226 83.4 131 272
loo gms. sat. solution of S in benzoyl chloride, C6H6.COC1, contain i gm. S at
o° and 55.8 gms. at 134°. (Bogousky, 1905.)
SOLUBILITY OF OCTOHEDRAL AND OF PRISMATIC SULFUR IN SEVERAL SOLVENTS.
(Brdnsted, 1906.)
The solubility of prismatic sulfur could not be determined in the ordinary way
on account of its rapid transition to octohedral sulfur. A special apparatus was
used which permitted the solvent to remain in contact with the solid for only a
short time. Since sulfur dissolves very rapidly, this procedure was found to give
satisfactory results. .
Gms. each Variety Separately per
100 cc. Saturated Solution.
Solvent. t°. . • TN
Prismatic Octohedral
Sulfur. Sulfur.
Benzene 18.6 2.004 1.512
25.3 2.335 I-835
Chloroform o i.ioi 0.788
15-5 1-658 1.253
40 2.9 2.4
Ethyl Ether o 0.113 0.080
25-3 0.253 0.200
Ethyl Bromide o 0.852 0.611
25.3 1.676 1.307
Ethyl Formate o 0.028 0.019
Ethyl Alcohol 25.3 o . 066 o . 05 2
703 SULFUR
SOLUBILITY OF SULFUR IN SEVERAL SOLVENTS.
Cms. S Cms. S
Solvent. t°. per 100 Gms. Solvent. t°. per 100 Gms.
Solvent. Solvent.
Aniline 130 85.3 (i) Glycerol 15.5 0.14(4)
Benzene 15.2 1.5 (2) Hydrazine (anhy.) room temp. 54(decomP.)(5)
19.3 1.7 (2) Lanoline (anhy.) 45 0.38(6)
26 0.97(1) Methylene Iodide 10 10 (7)
" 7i 4.38(1) Nicotine 100 10.6 (8)
Carbon Tetrachloride 25 0.86(3) Phenol 174 16.4 (i)
Chloroform 12.2 0.75(2) Pentachlor Ethane 25 1.2 (3)
19.3 0.92(2) Toluene 23 1.48(1)
22 1.21(1) Tetrachlor Ethane 25 1.23(3)
Dichlor Ethylene 25 1.28(3) Tetrachlor Ethylene 25 1.53(3)
Ethylene Chloride 25 0.84(3) Trichlor Ethylene 25 1.63(3)
Ethyl Ether 23.5 0.97(1) 15 1.16(9)
(i) Cossa, 1868; (2) Bronsted, 1906; (3) Hoffman, Kirmreuther and Thai, 1910; (4) Ossendowski, 1907;
(5) Welsh and Broderson, 1915; (6) Klose, 1907; (7) Retgers, 1893; (8) Kleven, 1872; (9) Wester and
Bruins, 1914.
SOLUBILITY OF SULFUR IN CARBON DISULFIDE.
(Etard, 1894; Cossa, 1865; at 10°, Retgers, 1893; below 77°, Arctowski, 1895-96.)
0 Gms. S per joo Gms. A0
Gms. S per 100 Gms. ^0
Gms. S per 100 Gms.
Solution.
CS2
Solution.
CS2.
Solution.
CS2. "
— no
3.0
3.1
— 10
*3-5
15-6
50
59-o
143.9
— 100
3-5
3-6
o
18.0
22 -O
60
66.0
194.1
- 80
4.0
4.2
10
23.0*
29.9
70
72.0
- 60
3-5
3-6
20
29-5
41.8
80
79.0
376.1
- 40
6.0
6.4
25
33-5
50-4
90
86.0
614.1
— 20
10.5
11.7
30
38.0
100
92 .0
1150.0
40
50.0
100 .0
* 26.4 R.
Sp. Gr. of solution saturated at 15° containing 26 gms. S per 100 gms. solution
= 1.372.
SOLUBILITY OF SULFUR IN HEXANE (C6Hi4).
(Etard.)
to Gms. S per to Gms. S per t<> Gms. S per
100 Gms. Solution. 100 Gms. Solution. 100 Gms. Solution.
— 20 0.07 60 i.o 130 5.2
o 0.16 80 1.7 140 6.0
20 0.25 100 2.8 160 7.2
40 0.55 120 4.4 180 8.2
SOLUBILITY OF SULFUR- (Sx) IN /3 NAPHTHOL, DETERMINED BY THE
SYNTHETIC METHOD.
(Smith, Holmes and Hall, 1905.)
The mixtures of sulfur and ft naphthol were heated until they were homo-
geneous and then cooled to the temperature at which clouding appeared.
t°of
Clouding.
Gms. S
per loo Gms.
0 Naphthol.
t°of
Clouding.
Gms. S
per 100 Gms.
0 Naphthol.
fof
Clouding.
Gms. S
per 100 Gms.
/3 Naphthol.
118
34
154
84.1
164
209.7
132.5
46.6
157
97-4
163-8
238.1
134-5
48.8
160.5
119.3
163-8
264.8*
143-5
59-3
162.5
145.1
I63
300*
149-5
70
163.5
177.6
* Solid phase, /3 naphthol.
SULFUR 704
CJLFUR IN COAL TAR Oi
(Pelouze, 1 86s
Grams S per 100 Grams Coal Tar Oil of: G S r 10
SOLUBILITY OF SULFUR IN COAL TAR OIL, LINSEED OIL AND IN OLIVE OIL.
(Pelouze, 1869; Pohl.)
4o Sp.Gr.: 0.87
* • b. pt.: 8o°-ioo°.
0.88
85°-i2o«.
0.882
I20°-220°
0.885
. I50°-200°
. 2IO°-300°
1.02
. 220°-300°.
OU' 0.885 Sp.Gr
15
2
.1
2.
3
2-5
2
.6
6.0
7.0
0-4
2-3
30
3
.0
4-
0
5-3
5
.8
8-5
8-S
0.6
4-3
SO
5
.2
6.
i
8-3
8
•7
IO.O
12 .O
I .2
9.0
80
ii
.8
13-
7
15-2
21
.0
37-o
41 -O
2 .2
18.0
100
15
.2
18.
7
23.0
26
•4
52-5
54-o
3'°
25.0
110
.
23-
o
26.2
31
.0
105.0
115.0
3-5
30.0
120
. .
.
27.
o
32-0
38
.0
00
00
4.2
37-o
130
.
.
38.7
43
.8
00
00
5-o
43-o
(160°)
10-0
100 gms. oil of turpentine dissolve 1.35 gms. S at 16°, and 16.2 gms. at b. pt.
(Payen, 1852.)
SOLUBILITY OF SULFUR IN TRIPHENYL METHANE, DETERMINED BY THE
SYNTHETIC METHOD.
Results of Smith, Holmes & Hall, 1905.
Results of Kruyt, 1908-09.
% Triphenyl
Methane in
t° of First
Limit of
% Triphenyl t° of Second
Methane in Limit of
% Triphenyl t° of First % Triphenyl
Methane in Limit of Methane in
t° of Second
Limit of
Mixture.
Mixing.
Mixture.
Mixing.
Mixture.
Mixing.
Mixture.
Mixing.
69.1
108.5
35-5
214.5
66.7
113
7
2II-5
58.8
127
32.5
211
60.2
125.3
9-3
201.5
50.8
136.5
28.4
506
5O. 2
136.8
12
198.8
46.6
141
24.5
203
41
144-2
13.7
199-5
42.8
144
21.6
200
30.8
I46
16.4
20O.4
37-8
146
19.2
199
2O
145-2
19.8
2O2. I
33-7
146.5
15.4
I98
13-2
137.6
23-5
203.7
30-3
147
8.1
II8.6
28.7
208
25.4
146
7
crystals
34-5
215.2
SOLUBILITY OF SULFUR IN PHENOL, DETERMINED BY THE SYNTHETIC METHOD.
(Smith, Holmes and Hall, 1905.)
f he mixtures of sulfur and phenol were heated until they were homogeneous
and then cooled to the temperature at which clouding appeared.
+0 £ Gms. S per t<> f Gms. S per to e Gms. S per
Clouding. 'ojGg-. Clouding. '~£f Clouding. '~£f
89.5 9.1 155 26.3 166 31.6
96.5 10.4 157.5 27.1 167.5 32.4
122.5 15.3 160.5 28.6 170 33.5
138 19.9 162 29.6 172 34.9
148.5 23.6 164.5 30-7 J75 36.5
RECIPROCAL SOLUBILITY OF SULFUR AND TOLUENE, DETERMINED BY THE
SYNTHETIC METHOD.
(Kruyt, 1908-09.)
Wt. % S in Limiting t" of Homogeneity. \yt. % S in Limiting t° of Homogeneity.
Mixture. Lower. Upper. " Mixture. ' Lower. Upper.
50.5 167 250 75.7 178 221
62 179 223 77.9 174
69.6 l8o 222 83.3 l6o 223
73 180 222 90.5 124 above 250
70S
SULFUR
RECIPROCAL SOLUBILITY OF SULFUR AND META XYLENE, DETERMINED
BY THE SYNTHETIC METHOD.
(Kruyt, 1908-09.)
Wt. % S in
Mixture.
50-9
49.1
47-7
44.2
40.4
Limiting t° i
af Homogeneity.
Lower.
181
177
172.5
161.5
153-5
Upper.
213
228
none (?)
" (255)
" (215)
Wt. % S in
Mixture.
39-9
84.2
86.1
87
90
Limiting t° of Homogeneity.
Lower.
152
none
164.5
159
139
Upper.
none (230)
«
199
202.5
none (220)
Fusion-point data for the system sulfur-tellurium are given by Pelabon (1909);
Pellini (1909); Chikashige (1911, 1911-12); Jaeger and Menke (1912).
Data for mixtures of sulfur and each of the following metals are given by Pela-
bon (1909); antimony, tin, lead, silver, gold and arsenic.
SULFUR DIOXIDE SO2
SOLUBILITY IN WATER.
(Schonfeld, 1855; Sims, 1861; Roozeboom, 1884.)
Schonfeld. Sims.
Vols. SO2 (at o° and Cms. SO2 per „ ~
760 mm.) per i Vol. I00 Cms? HaO SO2 per i Gm. H2O.
Roozeboom.
S02 Dissolved
peript.HaO
*•. Sat. SO,
+ Aq.
H20.
at total pressure t ».
760 mm.
Cms.
Vols.'
t .
Ul /LKJ Ullll.
pressure.
O
68
.86
79
•79
22
.83
8
0.168
58.7
O
0.236
5
59
.82
67
.48
19
10
0.154
53-9
2
0.218
10
51
•38
56
•65
16
.21
14
0.130
45-6
4
0.201
15
43
•56
47
.28
!3
•54
20
O.IO4
36-4
6
0.184
2O
36
.21
39
•37
II
•29
26
0.087
30-5
7
0.176
25
30
•77
32
•79
9
.41
30
0-078
27-3
8
0.168
30
25
.82
27
.16
7
.81
36
0.065
22.8
10
0.154
35
21
•23
22
•49
40
0.058
20.4
40
17
.01
18
•77
5
.41
46
0.050
17.4
12
0.142
50
0.045
15.6
Sp. Gr. of sat. solution at o° = 1.061; at 10°, 1.055; at 20° = 1.024.
The results of Sims are discussed and recalculated by Fulda, 1909.
I gm. H2O dissolves 0.0909 gm. SO2 = 34.73 cc. (measured at 25°) at 25° and
760 mm. pressure. (Walden and Centnerszwer, 1902-03.)
FREEZING-POINT DATA FOR THE SYSTEM SULFUR DIOXIDE — WATER.
Mols. SO,
VrLSLm I*51 I0° M°ls' Solid Phase-
Freezing. SO2+H2O.
O
O
Ice
— 0.2
0.8
"
-3 Eutec.
. . .
" +S02 Hydrate
— O.2
2.8
SO2 Hydrate
+3.5
3-3
"
6.8
5-5
"
(Baume and Tykociner, 1914.)
t°of
Freezing.
7-7
8-3
9-3
12. I
12.2
Mols. SOj
per loo Mols.
Solid Phase.
SO, Hydrate
5-9
ii
95-1
At the temperature +12.1° and extending over the range of concentration n
to 95.1 mols. per cent SO2 a second phase rich in SO2 separates. This crystal-
lizes at —74° and the diagram is consequently composed of two lines parallel to
the axis of concentration, the one at the +12.1° level corresponding to the SO2
hydrate, and the other at the —74° level, to the SO2 rich phase. The diagram is
terminated by a very short branch rising from —74° to the temperature of solidi-
fication of pure SO2 (—72.3°).
SULFUR DIOXIDE 706
SOLUBILITY OF SULFUR DIOXIDE IN WATER AT DIFFERENT PRESSURES.
(Lindner, 1912.)
Results at o°. Results at 25°. Results at 50°.
mm-Hg- ^ItVsoL0' mm. Hg. ^af.^oT nxm. Hg. 'sLufe?'
0.4 0.0537 i-4 0.0534 4.9 0.0525
3-5 0.237 n-75 0.234 30.5 0.2276
29.4 1.227 87.9 I. 212 204.5 I.lSl
109.4 3.804 313 3.750 696 3.628
SOLUBILITY OF SULFUR DIOXIDE IN AQUEOUS SALT SOLUTIONS.
(Fox, 1902.)
Results in terms of the Ostwald Solubility Expression. See p. 227.
A SoJubility Coefficient / of SO2 in aq. Solutions of Concentrations:
Aqueous A
Salt Solution. r0.s Normal 1.0 N. i.±V. 2.0 N. 2.5 N. 3-0 N?
NH4C1 £35=34-58 36-37 38-06 39.76 41.37 42.78
NH4Br £35=36-25 39.46 42.78 46.06 49.17 52.25
NH4CNS £35=37-78 42.74 47.26 52.26 57.01 61.46
NH4NO3 £35=33-96 35-o7 36-28 37.27 38.01 39.14
NH4NO3 £35=23-35 24-23 24.78 25.57 26.66 27.43
(NH4)2SO4 £35=33-35 33 -82 34-33 34-95 35-47 35-96
(NH4)2SO4 /35=22.9i 23.14 23.49 23.93 24.23 24.60
/25=3i.66 30.55 29.46 28.16 27.09 26.06
£35=2! -73 21.23 20.55 20.02 19.23 18.68
CdBr2 /25=3i.9i 31.01 30.17 29.27 28.15 27.46
CdBr2 /35=2i.88 21.46 20.81 20.60 19-70 19-17
CdI2 £25=33-27 33-76 34.16 34.74 34.98 35.77
CdI2 /35=22.75 23.06 23.36 23.71 23.99 24.30
CdSO4 /25=3i.ii 29.71 28.24 26.58 25.14 23.76
CdSO4 /35=2i.45 20.43 19-42 18-31 17-41 16.25
£25=34-42 36-05 37-76 39.32 40.96 42.27
£35=23-74 25.15 26.54 27.94 28.93 30.02
KBr £25=35-94 39 -11 42-41 44-96 48-87 52.26
KBr /35=24.83 27.49 29.64 31.93 34.12 36.14
KCNS £25=37-57 42-38 47 -02 51.81 55.87 61.26
KCNS £35=25-63 28.79 32-03 35-05 38.13 42.94
/25=38.66 44-76 50-58 56-75 62.63 68.36
£35=26.30 30.25 34-64 38.04 41-87 45-43
KNO, £35=33-80 34-79 35-77 36-66 37.57 38.52
KNO3 £35=23.27 24.03 24.79 25.72 26.54 27.33
K2SO4 £35=33-20 33.61
NaBr £25=33-76 34-54 35-27 36-26 36.84 37.74
NaCl 735=32.46 32.25 31.96 31.76 31.51 31.36
NaCNS £35=35-44 38-24 40-78 43-37 45-86 48-34
Na2SO4 /25=3i. 96 31.14 30.45 29.51 28.66 28.44
Na^C^ /35=2i.88 21.35 20.81 20.21 19.75 19-27
The author also gives a series of determinations in which a mixture of SO2 + CO2
is used for saturating the solutions, thus changing the concentration of the SO2
and yielding results for certain partial pressures of this gas.
m Additional data for the solubility of sulfur dioxide in aqueous salt solutions are
given by Walden and Centnerszwer (1902-03) but these authors present their
results in terms of the difference between the amount of SO2 dissolved in water
and in the aqueous solution. The exact manner in which these calculations were
made is not clearly explained.
707
SULFUR DIOXIDE
SOLUBILITY OF SULFUR DIOXIDE IN SULFURIC ACID OF 1.84 SP. GR.
Interpolated from original results.
o
10
20
25
30
40
Sp. Gr.
Coefficient
of Sat.
of Absorp-
t ° .
Solution.
tion (760 mm.).
53-o
50
1.8232
35-o
60
1.8225
25 .0
70
I .8221
21 -O
80
I.82I6
18.0
90
1.8205
13.0
(Dunn, 1882.)
Sp. Gr.
Coefficient
of Sat.
of Absorp-
Solution.
tion (760 mm.)
I. 8l86
9-5
1.8165
7.0
I.8l40
5-5
1.8112
4-5
I. 8080
4-0
SOLUBILITY OF SULFUR DIOXIDE IN AQUEOUS SULFURIC ACID SOLUTIONS.
(Dunn; see also Kolb, 1872.)
Sp. Gr. of
Approximate
Coefficient
<
>p. Gr. of
Approximate
Coefficient
t °
H2SO4
Per cent
of
t °«
H2SO4
per cent
of
Solution.
H2S04.
Absorption.
Solution.
H2S04.
Absorptior
6
9
•139
20
48.67
15
2
i
•173
25
31.82
6
9
• 300
40
4S-38
16
8
X
•I5I
21
3I-56
8
.6
.482
58
39 -91
14
8
z
.277
36
30.41
9
.8
•703
78
29.03
15
.1
I
•458
S^
29.87
5
•5
.067
10
36.78
15
.6
I
.609
70
25-I7
6
.0
.102
15
3.408
15
0
I
•739
81
20.83
For definition of Coefficient of Absorption, see Ethane p. 285.
SOLUBILITY OF SULFUR DIOXIDE IN ALCOHOLS AND IN OTHER SOLVENTS.
(de Bruyn, 1892; Schulze, 1881.)
In Ethyl Alcohol
at 760 mm.
o Gms. SO2 per 100 Gms.
In Methyl Alcohol
at 760 mm.
Gms. SO2 per 100 Gms.
Solution.
C2HsOH. Solution.
CH3OH.
0
53
•5
115
.0
71.1
246
.0
7
45
•o
8l
.0
59-9
149
•4
12
•3
39
•9
66
•4
52.2
109
.2
18
.2
32
.8
48
.8
(17. 8°) 44-0
78
,6
26
• O
24
4
32
•3
3I-7
46
•4
In Several Solvents
at o° and 725 mm. (S.)
S lve~t SO2 per i Gm. Solvent
Grams. Vols.
Camphor o . 880 308
CH3COOH 0.961 318
HCOOH 0.821 351
(CH3)2CO 2.07 589
SO2C12 0.323 189
SOLUBILITY OF SULFUR DIOXIDE IN CHLOROFORM.
(Lindner, 1912.)
Results at o^ Results at 25°.
Pressure in
mm. Hg.
Gms. SO;
per 100 cc
Sat. Sol.
2.7
5-6
22
O.O7OI
0.1790
0.6982
90.2
219.6
3-097
8.217
Pressure in
mm. Hg.
5-7
12.9
48
200.2
488.8
Gms. SOz
per 100 cc.
Sat. Sol.
0.0669
O.I7I2
0.6728
2-954
SULFUR DIOXIDE
708
SOLUBILITY OF SULFUR DIOXIDE IN SEVERAL SOLVENTS.
(Lloyd, 1918.)
The dry, air free, SO2 was passed through the solvent until saturation was
reached and 5 cc. (usually) of the saturated solution were mixed with a large volume
of water and titrated with standardized iodine solution.
Gms. SO2 per Liter of Saturated Solution in:
- 5
o
+ 5
10
15
20
25
3°
40
50
00
Benzene.
Nitro-
benzene.
Toluene.
o Nitro-
toluene.
Acetic
Anhydride.
. . .
196
148(^=1.22)
136
. . .
. . .
. . .
122
3II-4
. . .
290.8
114
267.4
217-5
236
106
227.9
170.4
192.2
99
127.5
190
124.4
160.7
90
82.9
I32
93-6
II8.5
. . .
60.3
98.7
77.2
87.2
. . .
34
78.6
54-7
68.8
DISTRIBUTION OF SULPHUR DIOXIDE AT 20° BETWEEN:
(McCrae and Wilson, 1903.)
Water and Chloroform.
Aq. HC1 and Chloroform.
Cms. SOa per
Liter in:
Gm. Equiv. iSO2
per Liter in:
Cone.
Gms. SOa per
Liter in:
Gm. Equiv. iSO2
per Liter in:
Aq.
Layer.
CHC13
Layer.
Aq.
Layer.
CHC13
Layer.
of
HC1.
Aq.
Layer.
CHC13
Layer.
Aq.
Layer.
CHC13
Layer.
I-738
I
.123
0
•0543
0
•0351
0.05
1.86
I .46
0-0581
0.0456
i-753
J.
.122
0
•0547
O
•0350
it
3-07
2.83
0-0960
0.0884
2.346
I
•703
0
.0732
0
•0532
ti
4.28
4.07
0.1336
O.I27I
2.628
I
.897
0
.082I
0
.0592
tt
5-34
,5.42
0-1667
0.1692
3-058
2
.385
0
•0955
0
•0745
0.10
1-25
I.4I
0-039
O.O44
3-735
3
.062
0
.1166
0
.0956
«
2.78
3.08
0.0868
0.0962
4.226
3
.626
0
'W9
0
.1132
«
3.86
4.08
0.1199
0-1275
5.269
4
.798
0
.1645
0
.1498
a
5.161
5-72
0.1612
0.1784
6.588
6
.I83
0
.2057
0
.1930
0.2
1.268
I-5I
0.0396
0.0471
31.92
33
.84
0
.9968
I
.056
if
1.914
2 .27
0.0597
O.O7lo
33-26
37
•25
I
.038
I
.163
(I
2.464
3-°4
0.0769
0-0949
a
3-967
4.90
0.1239
0-I530
0-4
i .202
1.61
0.038
0.0504
it
1.894
2 .26
0.059
0-0706
Freezing-point data for mixtures of sulfur dioxide and sulf uryl chloride (SO2C12)
are given by van der Goot (1913).
SULFURIC ACID H2SO4 (Sulfur Trioxide, SO3).
SOLUBILITY IN WATER.
(Landoldt and Bornstein, "Tabellen," 4th Ed., pp. 472-3, 1912.)
The available data for the freezing-points of mixtures of sulfuric acid and water
have been plotted and the most probable values read from the curves. The data
are also calculated to SO8. The complete results are given on the following page.
709
SULFURIC ACID
SOLUBILITY OF SULFURIC ACID IN WATER, DETERMINED BY THE
FREEZING-POINT METHOD.
Gms.
Gms.
H2S04
Gms. SO4
H2S04 Gms. S(
\
t°.
per 100
per 100 Gms. Solid Phase. t°.
per 100 per 100 Gms. Solid Phase.
Gms.
Sat. Sol.
Gms. Sat. So
1.
Sat. Sol.
Sat. Sol.
IO
16.25
l3-25(i) (S) . Ice
— IO
77-75 63.5 (3) SO,.2H20
20
24
i9-5(i)(
2) (3) "
0
80.25 65.5 (2)
30
28.5
23-25 (2)
+ 8.35
* 84-5 68.98 (2)
40
3I-25
25-5 (2) . "
8.81
84.5 68.98
i
50
33-5
27.25(l)
(2)
o
88.25 72
2
60
35-25
28.75 «
"
— 20
91-5 74-75
«
70
36.75
30 (2)
-30
92-5 75-5 (
75
38
31 (2) " +S03.SH20
-38
93 76 (2) "+S03.H20
70
39
31.75(2) S03.SH20
-30
93-75 76.5 (4) S03.H20
60
4i.5 33-75(2) '
— 20
95-25 77.75 (4)
50
44
36 (2) •
— IO
96.25 78.5 (i)(4) "
40
47-75
39 (2) "
o
97-75 79-75 (4)
30
53-25
43-25 (2) "
+ 10
99.75 81 (4)
25*
57.65
47.06 (2) " 10.35
100 81.62 (i)(3) (7X4)
30
61
49-75 (2) "
10
... 82 (4) «'
40
65-25
53-25 (2) "
0
• • • 83.25 (4) "
60
70.75
57-75 (3) " (unstable)
— IO
... 84.5 (4) "
70
73-25
59-75(3) " " +S03.2H20
— 12
85 (4) "+S03.*H20
60
73-50
60 (3
SO3.2H2O (unstable)
— IO
85.25 (4) S03.*H20
50
74-25
60.5 (3
Cl
O
... 86 (4)
50
68
55-5 (2
SO3.sH2O+SO3.3H2O
+ 10
. . . 86.75 (4)
45
68.5
56 (6
SO3.3H2O
20
... 87.5 (4)
40
58 (6) '•
3°
... 88.5 (4)
38.9*
73.M
59-69 (6) "
36*
. . . 89.89 (4)
40
74-25
60.5 (6) «
30
... 90-5 (4)
41
74-75
6 1 (6) " +SO3.2H2O
20
91.5 (4)
40
74-75
6 1 (4) SO3.2H2O
10
. . . 92.25 (4)
3°
75-25
6i-5 (4)
6.5
... 93 (4) " +(?)
20
76.5
62.5 (3).
* m. pt.
(i) =Pfaundler and Schnegg (1875); (2) = Pickering (1890); (3) = Thilo (1892); Pictet (1894); (4)
= Knietsch (1901); (5) = Rudorff (1862); (6) = Biron (1899); (7) = Marignac (1853). See also Pickering
(1890-91); Lespieau (1894) and Giran (1913).
SOLUBILITY OF SULFURIC ACID IN BENZENE SOLUTIONS OF VALERIC
ACID AT 1 8°.
(Gurwitsch, 1914.)
The mixtures were shaken with excess of 95.8% H2SC>4 at o° and then brought
to equilibrium at 1 8°.
Gms. Valeric
Acid per 100
Gms. Valeric
Acid+Benzene.
o=Pure benzene
0.584
1.62
3-64
7.60
17-5
Gms. H2S04
per 100 Gms.
of the
Sat. Solution.
O
0.052
O.IO4
0.226
0.378
0.454
TANNIC ACID 710
TANNIC ACID
When a sample of tannic acid of apparently very good quality was added to
water at room temperature, the solution increased so greatly in viscosity, that
even before the saturation point was reached, it became evident that a satisfac-
tory separation of liquid and solid could not be made. The solubility in water is
variously given in the pharmaceutical literature from about 20 to 300 gms. tannic
acid per 100 gms. of water. Similarly, the quoted results for the solubility in
alcohol vary from about 50 to 400 gms. acid per 100 gms. of alcohol. (Seidell, 1910.)
100 gms. glycerol dissolve 48.8 gms. tannin at 15-16°. (Ossendowski, 1907.)
100 gms. trichlorethylene dissolve 0.012 gm. tannin at 15°. (Wester and Bruins, 1914.)
TANTALUM Potassium FLUORIDE TaK2F7.
SOLUBILITY IN AQUEOUS HYDROFLUORIC AND POTASSIUM FLUORIDE SOLUTIONS.
(Ruff and Schiller, 1911.)
The tantalum salt was purified by repeated crystallizations from pure anhydrous
HF1. After drying at 120°, it was shaken in platinum flasks for 3 hour periods at
constant temperature with HF1 or KF1 solutions or both together. The saturated
solutions were filtered by means of a platinum funnel and subjected to analysis.
Mixture Shaken
in Pt. Flask.
K2TaF7+H2O
" +aq.4.77%KF
" +aq. 7-35% KF
" +aq.4.47%HF
" +aq. 4-2 %HF
" +aq. 24.3 %HF
" +aq. 10.44% HF+ ?
2I.92%KF $
" +H20
' +aq. 4-77% KF
' +aq.4.47%HF
' +aq. 4-2 %HF
' +aq. 23.3 %HF
' +aq. 21.92% KF-f
10.44% HF
The solid phases were identified only by their crystal forms and it is possible
that still others may be present.
TaH5.
KF.
HF.
OU11U JTilclbC.
i8
0.25
O.I2
O.O29
KzTayOzF«+K2TaF
18
0. 10
4-79
0.074
"
16
0.09
6-73
0.015
"
18
1.33
0.56
4-47
K2TaF7
18.5
1.24
0.52
4-2
"
18
5-35
2.25
24-3
"
18
0.036
21.93
10.44
"
85
2.18
1.69
0.85
K*Ta,AFM+K2TaF7
85
0.96
5-27
1.17
"
90
5-73
2.41
4-47
K2TaF7
90
6
2.52
4.2
"
90
10.9
4-59
24-3
"
90
1.18
22.42
10.44
"
TARTARIC ACIDS C2H2(OH)2(COOH)2. d, I, and racemic
SOLUBILITY OF EACH SEPARATELY IN WATER.
(Leidie,i882.)
t°. Grams Tartaric Acid per iooGms.'H2O. t°. Gms. Tartaric Acid per 100 Gms. H2O.
Dextro
Racemic
Racemic
Dextro
Racemic
Racemic
and Laevo
Ac.
Ac.
and Laevo
Ac.
Ac.
Acids.
Anhydrous.
Hydrated.
Acids.
Anhydrous.
Hydrated
o
115.04
8.l6
9-23
50
195.0
5O.O
59-54
10
125.72
12.32
I4.OO
60
217-55
64.52
78.33
20
139-44
18.0
20.6o
70
243 .66
80.56
99.88
25
147.44
21.4
24.61
80
273-33
98.12
124.56
30
156.2
25.2
29.10
•90
306.56
117 .20
I52-74
40
176.0
37-o
43-32
100
343-35
137.80
184.91
loo gms. H2O dissolve 140.8 gms. tartaric acid at 15
solution is 1.31.
0 The Sp. Gr. of the sat.
(Greenish and Smith, 1902.)
TARTARIC ACID
SOLUBILITY OF TARTARIC ACID IN ALCOHOLS.
(Timofeiew, 1894.)
Alcohol.
Methyl Alcohol
Ethyl Alcohol
r.
Gms. C2H2(OH)r
(COOH)2 M . ,
per 100 Gms.
t°.
per 100 Gms.
Solvent.
Solvent.
- 3
67.5 Ethyl Alcohol
+ 23
28.9
+ 19.2
70.1
39
31.8
23
73 . 2 Propyl Alcohol
- 3
8.74
39
77-3
+ 19
,2 10.85
- 3
22.4 "
23
11.85
+ 19.2
27.6
39
14.4
SOLUBILITY OF TARTARIC ACID IN AQUEOUS ETHYL ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1910.)
Wt. Percent j ,
C2HBOH cTsol
Gms. C2H2(OH)2(COOH)2
per loo Gms.
in Solvent.
Sat. Sol.
Solvent.
0
I.32I
57-9
137.5
IO
1.300
56
127.3
20
1.276
54-1
II7.9
30
I.25I
52
108.3
40
I.22O
49.6
98.4
50
I.I84
47
88.6
Wt. Per cent
Gms. C2H2(OH)2(COOH)2
per 100 Gms.
Solvent
Sat. Sol.
Solvent.
60
1.142
43.9
78-3
70
1.095
4O.2
66.9
80
1.040
35-3
54-6
90
0-973
29
40.8
95
0-937
25-4
34-1
IOO
0.905
21.6
27.6
SOLUBILITY OF TARTARIC ACID IN SEVERAL SOLVENTS.
Solvent.
Amyl Alcohol
Benzene
Carbon Tetrachloride
Ether
u
Dichlorethylene
Trichlorethylene
Sp. Gr. of
Solvent.
<*25 Of
Sat. Sol.
Gms. C2H2(OH)2-
t°. (COOH)2 per 100 Authority.
Gms. Solvent.
^20 = 0.817
f/25 = 0.873
dz^ — 1.587
dzz = 0.711
0.824
0.875
1.589
0.715
25
25
25
25
3 . 50 (Seidell, 1910.)
0.0086
0.0189
O.6l "
15
0 . 40 (Bourgoin, 1878.)
IS
0 . 005 (Wester & Bruins, '14.)
15
O.O05
DISTRIBUTION OF TARTARIC ACID BETWEEN WATER AND ETHER.
Results at 15°.
Gms. Mols. per Liter.
(Pinnow, 1915.)
H2O Layer, c.
I.4O2
0.790
0.446
Ether Layer, c'
O.OO72
0.0037
O.OO22
Results at 27°.
Gms. Mols. per Liter.
197
2l6
2IO
H2O Layer, c.
1.625
0.857
0.427
Ether Layer, c'.
0.0070
0.0033
0.0016
233
259
268
F.-pt. data are given for mixtures of the d and racemic modifications of dimethyl
ether of tartaric acid, and for mixtures of the d and racemic modifications of di-
methyl ether of diacetyl tartaric acid by Roozeboom (1899). Results for mixtures
of the d and * forms of the diformalic derivative of racemic tartaric acid by Ringer
(1902). Results for mixtures of d tartaric acid and racemic acid ester and for d
diacetyl tartrate and racemic acid ester are given by Beck (1904). Data for
mixtures of d and / tartaric acid and for mixtures of d and i dimethyl ester of tar-
taric acid are given by Centnerszwer (1899).
PyroTARTARIC ACID (Methyl Succinic Acid) CH3.CH(COOH).CH2(COOH).
loo gms. H2O dissolve 51 gms. CH3CH(COOH).CH2COOH at 19.5°.
(Timofei
imofeiew, 1894.)
PyroTARTARIC ACID
712
Alcohol.
t°.
Gms. Acid
per loo Gms
Solvent.
Methyl Alcohol
— 18.5
53
tt
+19
109.8
ii
+ I9-S
II2.5
Ethyl Alcohol
+ 19
70.8
SOLUBILITY IN ALCOHOLS.
(Timofeiew, 1894.)
Alcohol.
Ethyl Alcohol 19
Propyl Alcohol 19
5
iQ-5
Gms. Acia
per 100 Gms.
Solvent.
72.4
44-9
47.1
100 gms. 95% formic acid dissolve 17.8 gms. pyrotartaric acid at 18.5°.
(Aschan, 1913.)
TERPIN HYDRATE Ci0H18(OH)2.HsO.
100 cc. H2O dissolve 0.36 gm. terpin hydrate at 15-20°. .
100 cc. 90% alcohol dissolve 7.1 gms. terpin hydrate at 15-20°.
(Squire and Caines, 1905.)
TELLURIUM Te.
100 gms. methylene iodide, CH2l2, dissolve o.i gm. Te at 12°. (Retgers, 1893.)
DISTRIBUTION OF TELLURIUM BETWEEN AQUEOUS HYDROCHLORIC ACID AND
ETHER AT ROOM TEMPERATURE.
(Mylius, 1911.)
When i gm. of tellurium as the chloride, TeCU, is dissolved in 100 cc. of aqueous
HC1 and shaken with 100 cc. of ether, the following per cents of the metal enter
the ethereal layers. With 20% HC1, 34 per cent; 15% HC1, 12 per cent; 10%
HC1, 3 per cent; 5% HC1, 0.2 per cent and with i% HC1, only a trace of the
tellurium.
Fusion-point curves for mixtures of tellurium and each of the following metals
are given by Pelabon (1909) : Sb, Sn, Pb, Ag, Au and As. Results for mixtures of
Te and Zn are given by Kobayashi (1911-12).
Mols.
"ss^r
H20.
4.67 H2Te04.2H20
5-33
7.04
9-93
14.52
19
TELLURIUM DOUBLE SALTS
SOLUBILITY OF TELLURIUM DOUBLE BROMIDES AND CHLORIDES IN AQUEOUS
HYDROCHLORIC AND HYDROBROMIC ACIDS AT 22°.
(Wheeler,
TELLURIC ACID H2TeO4.2H2O.
SOLUBILITY IN WATER.
(Mylius, 1901.)
Gms. Mols.
Gms.
t°.
H2TeO4 per H2TeO4 pe
100 Gms. 100 Mols.
r Solid Phase.
t°.
H2TeO4 per
100 Gms.
Sol. H2O.
Sol.
0
13.92 1.51
H2TeO4.6H2O
30
33.36
5
17.84 2.03
"
40
36.38
10
26.21 3.31
«
60
15
32.79 4-55
«
80
S'-SS
10
25-29 3-15
H2TeO4.2H2O
100
60.84
18
28.90 3.82
"
no
67
Tellurium Double Salt.
Formula.
Solvent.
Gms. Double Salt per too
Gms. Solvent
Te Caesium Bromide TeBr4.2CsBr Aq. HBr
Te Potassium Bromide TeBr4.2KBr
Te Rubidium Bromide
Te Caesium Chloride
Te Rubidium Chloride
TeBr4.2RbBr "
TeCl4.2CsCl Aq. HC1*
TeCl4.2RbCl
of i .49 Sp. Gr.
of i .08 Sp. Gr.
O-O2
0.13
6-57
62.90
0.25
3-88
0.05
0.78
o-34
13.09
• Sp. Gr. of Aq. HC1 solutions 1.2 and 1.05 respectively.
TELLURIUM IODIDE
TELLURIUM TetralODIDE TeI4.
SOLUBILITY IN MIXTURES OF AQUEOUS HYDRIODIC ACID AND IODINE AT 25°.
(Menke, 1912.)
Weighed amounts of TeL + 1+65 wt. % HI solution were shaken in sealed
glass tubes for 10 days. Both the clear saturated solution and the solid phase
were analyzed.
Solid Phase.
Small amt. TeL..HI.8HaO
tiuch
t< «<
small amt. "
TeI<.HI.8H,0
Iodine
SOLUBILITY IN WATER AT 25°.
(Locke, 1901.)
Salt per 100 Grams HjO.
Composition of Original Mixture
in Gms.
Gms. per 100 Gms.
Solution.
TeL..
i.
64% HI.
• Tel*.
i.
3
i-5
I9-25
12
11.7
2
o-5
9.61
13
o
2
o-S
9.61
13-5
8.2
3
3
8.99
20
21.8
Excess
None
5 (cc-)
9
0.19
2
9
9.10
IO
52.4
4
10
9.27
15
47-7
3
7
9.02
J7-5
47-9
None
Excess
5 (cc.)
None
61.1
THALLIUM ALUMS
Alum.
Formula.
Tl Aluminum Alum
Tl Vanadium Alum
Tl Chromium Alum
Tl Iron Alum
See also pp. 31 and 32.
TlAl(S04)2.i2H20
TlV(S04)2.i2H00
TlCr(S04)2.i2H20
TlFe(S04)2.i2H20
Gms.
Gms.
Gm.
Anhydrous.
Hydrated.
Mols.
7-5
11.78
0.0177
25.6
43-31
0-0573
10.48
16.38
0.0212
36-I5
64.6
0.0799
THALLIUM BROMATE TlBrO3.
One liter saturated aqueous solution contains 3.463 gms. TIBrOs at 19.9° (B6tt-
ger, 1903) and 7.355 gms. at 39.75°. (Noyes and Abbot, 1895.)
THALLIUM BROMIDE TIBr.
One liter sat. aqueous solution contains 0.238 gm. TIBr at 0.13°, 0.289 gm- a*
9.37°, 0.4233 gm. at 1 8° and 0.579 gm. at 25.68°. (Kohlrausch, 1908.)
SOLUBILITY OF THALLIUM BROMIDE IN AQUEOUS SOLUTIONS OF THALLIUM
NITRATE AT 68.5°.
(Noyes, 1890.)
Gms. Mols. per Liter. Gms. per Liter.
T1NO3.
O
0.0163
0.0294
0-0955
TIBr.
0.00869
O.OO4IO
0.00289
O.OOI48
T1NO3.
O
4.336
7.820
25.400
TIBr.
2.469
I.l64
0.821
0.420
F.-pt. data for mixtures of TIBr + T1C1, TIBr + Til and T1C1 + Til are given
by Monkemeyer (1906). Results for T1C1 + SnCl2 and T1C1 + ZnCl2 are given
by Korreng (1914).
THALLIUM, CARBONATE T12C03.
SOLUBILITY IN WATER.
(Crookes, 1864; Lamy, 1863.)
t°. 15.5°- 18°. 62°. 100°. 100.8°.
Gms. T12CO3 per 100 gms* H20 4.2 (C.) 5.23 12.85 27-2 (C.) 22.4
THALLIUM CHLORATE 714
THALLIUM CHLORATE T1C1O3.
SOLUBILITY IN WATER.
(Muir, 1876.)
t°. 0°. 20°. 50°. 80°. 100°.
Gms. TIClOs per ioo gms. H2O 2 3.92 12.67 36-65 57.31
One liter sat. aq. solution contains 38.51 gms. T1C1O3 at 20°. (Noyes and Parrel, 1911.)
One liter of aqueous solution, saturated with both salts, contains 30.4 gms.
TIClOa + 3443 gms. T12SO4 at 2O°. (Noyes and Farrel, 1911.)
SOLUBILITY OF MIXED CRYSTALS OF THALLIUM CHLORATE AND POTASSIUM
CHLORATE IN WATER AT 10°.
(Roozeboom, 1891.)
NOTE. — Solutions of the two salts were mixed in different proportions and
allowed to crystallize, such amounts being taken that not more than one or two
grams would separate from one liter.
Gms. per 1000 cc. Mg. Mols. per 1000 cc. Sp. Gr. Mols. per cent
Solution. ^ Solution. of KC1O3 in Mixed
'T1C1O3. KC1O3. T1C1O3. KC1O3. Solutions. Crystals.
25-637 ••• 89.14 ... I.O2IO O
19.637 6.884 68.27 56.15 I.O222 2
12.001 26.100 41.73 212.89 1.0278 12. 6l
9.036 40.064 3I-42 326.79 i -0338 25.01
7.885 46.497 27.42 379.26 1.0359 > 36.30_97
7.935 46.535 27.60 379-57 1.0360 ) *
6.706 46.410 23.32 378.55 1-0357 99-28
6.723 47-109 23.37 384-25 1-0363 99.60
4.858 47-312 16.89 385-91 1-0345 99-62
2.769 47-134 9-63 384.46 1.0330 99.67
49.925 ... 407.22 1.0330 ioo
SOLUBILITY OF MIXED CRYSTALS OF THALLIUM CHLORATE AND POTASSIUM
CHLORATE IN WATER AT -DIFFERENT TEMPERATURES.
(Quoted by Rabe, 1902.)
ioo gms. H2O dissolve 2.8 gms. T1C1O3 + 3.3 gms. KC1O3 at o°.
H2O dissolve 10 gms. T1C1O3 + 1.5 gms. KC1O3 at 15°.
H2O dissolve 12.67 gms. T1C1O3 + 16.2 gms. KC1O3 at 50°.
H2O dissolve 57.3 gms. T1C1O3 + 48.2 gms. KC1O3 at 100°.
THALLIUM PerCHLORATE T1C1O4.
SOLUBILITY IN WATER.
(Carlson, 1910.)
c n Gms. T1C1O4 c r Gms. T1C1O4 per
t°. IP-^J per ioo Gms. t°. Jg-gS ioo Gms.
H20. Sat' SoL H20.
o i. 060 6 50 1.251 39-62
10 1.075 8.04 70 1.430 65.32
30 1.146 I9.72 80 L520 81.49
ioo gms. H2O dissolve 10 gms. T1C104 at 15° and 166.6 gms. at 100°.
(Roscoe, 1866.)
715
THALLIUM CHLORIDE
THALLIUM CHLORIDE T1C1.
SOLUBILITY IN WATER.
(Average curve from results of Noyes, 1892; Bottger, 1903; Kohlrausch, 1904; Hebberling; Crookes;
Lamy. The results of Berkeley, 1904 are also given.)
jo^ Cms. T1C1 per Liter.
o 2.1 (av.) 1.7 (B.)
10 2.5 2.4
20 3.3 3-4
t°.
25
30
40
50
Gms. T1C1 per Liter
. t°. Gms- T1C1 per Liter.
3-86
4.2
5-2
6-3
4
4.6
6
8
60
80
IOO
8
12
18
IO.2
16
24.1
(99.3°)
The results of Berkeley are in terms of gms. of T1C1 per 1000 gms. H2O but
since the densities of the solutions are approximately I in all cases, except for
temperatures above 60°, the differences are negligible. The Sp. Gr. of the sat.
sol. at 99.3° is 0.9787 and the figure 24.1, therefore, becomes 23.58 gms. per liter.
One liter sat. solution in water contains 2.27 gms. T1C1 at 9.54°, 3.05 gms. at
17.7°, and 3.97 gms. at 25.76°. (Kohlrausch, 1908.)
SOLUBILITY OF THALLIUM CHLORIDE AT 25° IN AQUEOUS SOLUTIONS OF:
Nitric Acid.
(Hill and Simmons, 1909.)
Normality of
Aq. CHsCOOH
0
0.0501
0.0958
0.263
0.524
Acetic Acid.
(Hill, 1917.)
T1C1 per Liter.
•• Gms.
3.8515
3.8375
3.8326
3.7503
3.6539
Gm. Equiv.
O.Ol6o85
O.OI6027
O.Ol6oo6
0.015662
0.015258
Normality of d^ of
Aq. HN03. Sat. Sol.
o 0.996
0.4977 1.0184
1.0046 1.0359
T1C1 per Liter.
'Gms. Gm. Equiv."
3.951 0.0165
5-937 2.475
6.882 2.875
2.0452 1.0705
4.0170 1.1362
8.143 3-401
9.925 4.145
SOLUBILITY OF THALLIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SALTS
WITH A COMMON ION AT 25°.
(Noyes, 1892.)
Aqueous
Solution of:
Gms. Equiv.
Added Salt
per Liter.
Gms. Equiv.
Dissolved T1C1
per Liter. .
Water alone
O
o. 01612
NH4C1
0.025
0.00877
"
0.05
0.00593
"
0.20
O.0027I
BaCl2
0.05
O.OO62O
"
O.IO
0.00425
CdCl2
0.025
O.OI040
"
0.05
0.00780
"
O.IO
0.00578
tt
O.2O
0.00427
CaCl2
0.025
0.00899
"
0.05
0.00624
u
O. IO
0.00417
"
O. 2O
0.00284
CuCl2
0.025
0.00905
"
0.05
0.00614
tt
O.IO
O.OO422
tt
O.2O
O.OO29I
HC1
0.025
0.00869
"
0.05
0.00585
"
O.IO
0.00384
tt
O.2O
0.00254
Aqueous
Solution of:
Gms. Equiv.
Added Salt
per Liter.
Gms. Equiv.
Dissolved T1C1
per Liter.
MgCl2
0.025
o . 00904
u
0.050
0.0o6l8
"
O. 10
0.00413
tt
O.20
0.00275
MnCl2
0.025
0.00898
tt
0.05
0.00617
u
O.IO
O.OO4I2
u
O.2O
O.O0286
KC1
0.025
0.00872
u
0.05
0.00593
K
O.IO
0.00399
"
O.2O
O.O0265
tt
0.80
O.OOI70
NaCl
0.025
0.00869
tt
0.05
0.00592
tt
O.IO
0.00395
(l
O.2O
O.OO27I
TIClOs
0.025
0.00897
tt
0.025
0.00894
T1N03
0.025
0.00883
tt
0.05
O.OO626
tt
O.IO
0.00423
THALLIUM CHLORIDE
716
SOLUBILITY OF THALLIUM CHLORIDE IN AQUEOUS SALT SOLUTIONS AT 25°.
(Noyes, 1890; Noyes and Abbott, 1895; Geffcken, 1904.)
Aq. Salt Solution.
Ammonium Nitrate NT^NOa
Barium Chloride BaCl2
u
Cadmium Sulfate CdSO4
u
II
Hydrochloric Acid HC1
Lithium Nitrate LiNO3
Potassium Chlorate KC103
Potassium Nitrate KNO8
Sodium Acetate CHsCOONa
Sodium Nitrate NaNOs
Sodium Chlorate NaClO«
Thallium BromateTlBrOs (at 39.75°)
ThaUium Nitrate T1NO3
ThaUium Sulfate T12SO4
ThaUium Thiocyanate T1SCN
(at 39.75°)
NOTE. — In the case of 'the results for thallium bromate and thallium thio-
cyanate at 39.75°, the solutions were saturated with respect to these salts as well
as with respect to thallium chloride.
G. Mols^per Liter.
Cms. per Liter.
' Salt.
T1C1. "
Salt.
T1C1. '
o
0.01612
0
3-86i(G.)
o-S
0.02587
40.02
6.209
i
0.03121
80.05
7-473
2
0.03966
160. 10
9-497
0.0283
0.00857
5-895
2.052 (N.)
0.1468
0.00323
30.59
0-773
0.030
0.0206
6.255
4-933(N.)
0.0787
0.0254
16.41
6.081
0.1574
0.0309
32.82
7-399
0.0283
0.00836
1.032
2.002 (N.)
0.0560
0.00565
2.043
1-353
0.1468
0.00316
5-357
0-757
o-5
0.02542
34-53
6.085 (G.)
i
0.03035
69.07
7.266
2
0.03785
138-14
9.063
3
0.04438
207.21
10.630
0-5
0.0237
61.28
5-674(0.)
0.015
0.0170
i.5i7
4.070 (N.)
0.030
0.0179
3-033
4.286
0.0787
0.0192
7.775
4-597
0.1574
0.0212
15-920
5.076
o-S
0.0257
50.55
6.i53(G.)
i
0.0308
IOI. II
7-375
2
0.0390
202.22
9-340
0.015
0.0168
I.23I
4.023 (N.)
0.030
0.0172
2.462
4.118
0.0787
0.0185
6.46
4-430
0.1574
0.0196
12.92
4-693
0-5
0.02564
42.50
6.i39(G.)
I
0.03054
85.01
7.313
2
0.03851
I7O.O2
9. 221
3
0.04544
255-03
10.88
4
0.05128
340.12
12.28
o.S
0.02320
53-25
5-555(G.)
i
0.02687
106.5
6-433
2
0.03060
213
7-326
3
0.03303
3I9-S
7.909
4
0.03850
426
9-215
0.01567
0.01959
5-201
4.690(N.&A.)
0.0283
0.0083
7.518
1.987 (N.)
0.0560
0.00571
14.89
1.368
0.1468
0.00332
39-05
0-795
0.0283
0.00886
14.27
2. 121 (N.)
0.0560
0.00624
28.23
1.494
0.0107
0.0119
2.802
2.849 (N.)
0.02149
0.01807
5.632
*.326(N.&A.)
717
THALLIUM CHLORIDE
SOLUBILITY OF THALLIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SALTS AT 25°
(Bray and Winninghoff, 1911.)
Solvent.
Saturated Solution.
Salt
Gms. Equiv.
dj>* of Aq.
Gms. Equiv.
dy. of Sat.
Gms. Equiv.
Present.
Salt, per Liter.
Solvent.
Salt per Liter.
Sol.
T1C1 per Liter.
None
. . .
0-9994
0.01607
KNO3
O.O200I
0.9973
O.020
I.OO09
0.01716
"
O.05000
0.9992
0.04997
1.0028
0.01826
"
0.10005
1.0023
0.09998
1.0063
0.01961
"
0.3002
I.OI45
0.3000
1.0194
0.02313
M
1.0005
1.0568
0.9996
1.0632
0.03072
K2SO4
0.01997
0.9975
0.01996
I. 0012
0.01779
(i
O.O5000
0.9995
0.04996
1.0037
0.01942
"
0. IOOO
1.0030
0.09989
1.0074
0.02137
"
0.3000
1.0167
0.29966
I.O22I
0.026OO
M
I
1.0628
0.9986
1.0698
0.03416
T12S04
0.02OO
I.OOO7
O.OI999
1.0028
0.01034
"
O.05OO
1.0076
0.04999
I . 0090
0.006772
"
O. IOOO
I.OI9I
0.09997
I.O200
o . 004679
One liter of water dissolves 2.7 gms. thallo thallic chloride 3T1C1.T1C13 at I5°-I7°,
and 35 gms. at IOO°. (Crookes, 1864; Lamy; Hebberling.)
THALLIUM CHROMATE Tl2CrO4.
100 gms. H2O dissolve 0.03 gm. Tl2CrO4 at 60°, and 0.2 gm. at 100°.
(Browning and Hutchins, 1900.)
One liter of aq. 31 per cent KOH solution dissolves 18 gms. Tl2CrO4.
(Lepierre and Lachand, 1891.)
One liter of H2O dissolves 0.35 gm. thallium trichromate, T^CrsOio, at 15°,
and 2.27 gms. at IOO°. (Crookes, 1864.)
THALLIUM CYANIDE T1CN and Double Cyanides.
SOLUBILITY IN WATER.
(Fronmtiller, 1878.)
Formula.
Cyanide.
Tl Cyanide T1CN
Tl Cobalti Cyanide Tl3Co(CN)6 3.6
Tl Zinc Cyanide 2TlCN.Zn(CN)2 8.7
Tl Ferro Cyanide Tl4Fe(CN)6.2H20
Gms. Salt per 100 Gms. H2O.
16.8 at 28.5°.
at oc
at o°; 15.2 at 14°; 29.6 at 31°.
0.37 at l8°; 3.93 at IOI°. (Lamy.)
5.86 at 9.5°; 10.04 at 19.5°
THALLIUM FLUORIDE TIP.
100 gms. H2O dissolve 80 gms. T1F at 15°.
THALLIUM HYDROXIDE T1OH.
(Bttchner, 1865.)
SOLUBILITY IN WATER.
(Bahr, 1911.)
to 4lB °f
Mols. T1OH
Gms. T10H
t°
Mols. T1OH
Gms. T1OH
Sat. Sol.
per Liter.
per Liter.
v *
per Liter.
per Liter.
O
.231
I.I5I
254-4
44-5
2.442
539-8
I8.5
.317
1.554
343-4
54-1
2.940
649.7
29
•342
1.803
398.5
64.6
3.601
795-8
32.1
•377
1.861
4II.2
78.5
4.673
1033
36
.417
2.075
458.6
90
5.705
1261
40
.446
2.240
495
99.2
6.708
1483
The solutions were stirred by means of a current of hydrogen. The solid phase
is the same at all temperatures.
THALLIUM IODATE 718
THALLIUM IODATE T1IO3.
One liter aq. solution contains 0.578 gm. T1IO3 at 20°. (Bottger, 1903.)
One liter aqueous solution contains 1.76.10^ mols. TlIOs at 25° = 0.667 gm-»
determined by means of electrodes of the third kind. (Spencer, 1912.)
THALLIUM IODIDE Til
One liter sat. solution in water contains 0.0362 gm. at 9.9°, 0.056 gm. at 18.1°
and 0.0847 Sm- at 26°. (Kohlrausch, 1908.)
SOLUBILITY OF THALLIUM IODIDE IN WATER.
(Average results from Bottger, 1903; Kohlrausch, 1904-05; Werther; Crookes, 1864; Lamy; Hebberling.)
t°. o°. 20°. 40°. 60°. . 80°. 100°.
Cms. Til per liter 0.02 0.06 0.15 0.35 0.70 1.20
One liter of 2^ per cent aq. ammonia dissolves 0.761 gm. T1C1.
One liter of 6^ per cent aq. ammonia dissolves 0.758 gm. T1C1.
One liter of 90 per cent alcohol dissolves 0.0038 gm. T1C1.
One liter of 50 per cent alcohol dissolves 0.027 gm> T1C1. (Long, 1888.)
Data for the temperatures of solidification of mixtures of Til and TINOs are
given by Van Eyk (1901).
THALLIUM NITRATE T1NO3.
SOLUBILITY IN WATER.
(Berkeley, 1904; see also Etard, 1894; Crookes; Lamy.)
e Gms. TINOa per 100 Cms. 0 Gms. TINOa per TOO Gms.
Solution. Water. Solution. Water.
o 3.76 3.91 60 31.55 46.2
10 5-86 6.22 70 41.01 69.5
10 8.72 9.55 80 52.6 in.o
30 12.51 14.3 90 66.66 200. o
40 17.33 20-9 I0° 8o-54 4i4-o
50 23.33 3o-4 105 85.59 594.0
Solid phase. TINOs rhombic.
loo gms. H2O dissolve 43.5 gms. T1NO3 + 104.2 gms. KNO8 at 58°. (Rabe, 1902.)
THALLIUM OXALATE T12C2O4.
One liter of saturated aqueous solution contains 15.77 gms. T12C2O4 at 20°, and
18.69 gins, at 25°. (Bottger, 1903; Abegg and Spencer, 1905.)
SOLUBILITY OF THALLIUM OXALATE AT 25° IN AQ. SOLUTIONS OF:
Thallium Nitrate.
(Abegg and Spencer.)
Mol. Concentration. Grams per Liter.
Potassium Oxalate.
(Abegg and Spencer.)
Mol. Concentration. Grams per Liter.
T1NO3.
0.0
O.O4II4
0.0799
o-i597
T12C204.
0.03768
0.0264
0.0195
0.01235
T1N03.
o.oo
10-95
21 .26
42.51
T12C204.
18.69
13.10
9.68
6.128
K2C204.
0-0498
0-0996
0.2467
0.4886
0.9785
T12C2O4.
0.0351
0-03565
0.0390
0-04506
0-05536
K2C204.
8.281
16.57
41 .02
81.25
162.6
T12C204.
17.42
17.69
19.36
22.37
27.48
THALLIUM PHOSPHATE (ortho) T13PO4.
One liter of sat. aqueous solution contains 4.97 gms. T13PO4 at 15° and 6.71
(Crookes, 1864.)
719
THALLIUM PICRATE
THALLIUM PICRATE T10C6H2(NO2)3.
SOLUBILITY IN WATER.
(Rabe, 1901.)
Cms.
T10C,H2(N02),
per 100 Gms.
H20.
0.135
0.36
o-575
Gms.
t,
Solid Phase.
Solid Phase.
o
18
30
40
47
Monoclinic Red
per ioo Gms.
H20.
1.04 Triclinic Yellow
1 . 10 "
1.205
0.825 " 60 1.73
2-43
ioo gms. H2O simultaneously sat. with both salts dissolve:
0.132 gm. C6H2(N02)3OT1 + 0.36 gm. C6H2(NO2)8OK at o°.
0.352 " + 0.44 " 15°.
0.38 +0.23 "20°. (Rabe, 1901.)
SOLUBILITY OF THALLIUM PICRATE IN METHYL ALCOHOL.
45
47
50
60
70
Gms.
t°.
TlOC,H2(NO2)s
per loo Gms.
CHjOH.
o
0.39 I
18
0-S9
25
0.70
30
o-795
35
0.90
40
i. 02
45
1.17
47
1.265
(Rabe, 1901.)
Solid Phase.
Red Form (monoclinic)
Gms.
to T10C,H2(NO2)8
per ioo Gms.
CH3OH.
45
-195
48
.265
50
•325
53
.41
57
•54
00
•65
65
.84
Solid Phase.
Yellow Form (triclinic)
THALLIUM SEI,ENATE Tl2SeO4.
SOLUBILITY IN WATER.
9-3
12
20
80
100
Gms. Tl2SeO4
per 100 Gms. H2O.
2.13
2.4
2.8
8-5
10.86
Authority.
(Tutton, 1907.)
(Glauser, 1910.)
«
(Tutton, 1907.)
THALLIUM SULFATE T12SO4.
SOLUBILITY IN WATER.
(Berkeley, 1904; see also Crookes; Lamy.)
Gms. TljiSC^ per 100 Gms.
i .
Solution.
Water.
0
2.63
2.70
IO
3-57
3-70
20
4.64
4.87
30
5.8o
6.16
50
8-44
9.21
I .
Solution.
Water.
60
9.89
10.92
70
II-3I
12.74
80
12.77
14.61
00
14.19
16.53
99-7
15-57
18.45
ioo gms. H2O dissolve 3.36 gms. T12SO4 at 6.5°, 4.3 gms. at 12° and 19.14 gms.
at 100°. (Tutton, 1907.)
One liter sat. solution in water contains 48.59 gms. T12SO4 at 20° (Noyes and
Farrel, 1911) and 54.59 gms. at 25° (Noyes and Stewart, 1911).
ioo gms. H2O simultaneously sat. with both salts dissolve:
4.74 gms. T12SO4 + 10.3 gms. K2SO4 at 15°.
11.5 " " + 16.4 62°.
18.52 " " +26.2 " 100°. (Rabe, 1902.)
THALLIUM SULFATE
720
SOLUBILITY OF THALLIUM SULFATE IN AQUEOUS SOLUTIONS AT 25°.
(Noyes and Stewart, 1911.)
Saturated Solution.
Solvent.
Salt Present.
T1NO3
Formula Wts.
Salt
per Liter.
tt
0.04995
O.2O
NaHSO4
H2SO4
O.IOI5
0.04967
"
0.09933
Formula Wts.
Formula Wts.
j _r
Gms.
Gms.
Salt
per Liter.
T12S04
per Liter.
Sat Sol.
Salt
per Liter.
T12S04
per Liter.
o . 0996
0.08365
. . .
26.51
42.17
0.0497
o . 1080
I-053I
7.062
54-44
0.1988
O.II73
1-0754
28.25
59-13
O.IOIO
0.1161
1.0596
12 .12
58.53
o . 0494
0.1172
I . 0540
4.878
59-09
0.0987
0.1249
I . 0604
9-747
62.95
SOLUBILITY OF THALLIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 25°.
(D'Ans and Fritsche, 1909.) •
' H2S04.
T12SO4. '
H2S04.
T12S04.
. ouiiu jriiasc.
0
0.103
T12S04
4.89
o-59
T1HS04
2.99
0.46
" +T13H(S04)2
4.92
0.66
"
4-25
0.61
T13H(S04)2+T1HS04
4.78
0-75
it
4-55
0.56
T1HSO,
4.26
1. 01
*
4-79
o-55
"
4-03
i. 08
•i
THALLIUM DOUBLE SULFATES
SOLUBILITY IN WATER AT 25°.
(Locke, 1901.)
Double Sulfate.
Tl Copper Sulfate
Tl Nickel Sulfate
Tl Zinc Sulfate
Formula.
Tl2Cu(SO4)2.6H2O
Tl2Ni(S04)2.6H20
Tl2Zn(SO4)2.6H2O
Salt per 100 cc. H2O.
Gms. Anhydrous. Gms. Mols.
8.1 O.OI22
4.6l O.OO7
8.6 0.0129
THALLIUM SULFIDE T12S.
One liter of sat. aqueous solution contains 0.215 gm- T12S at 20°. (Bottger, 1903.)
A diagram and discussion of the fusion points of T12S + S, T12S + Se and
T12S + Te are given by Pelabon, 1907.
(Seubert and Elten, 1892.)
THALLIUM SULFITE T12SO8.
100 gms. H2O dissolve 3.34 gms. T12SO3 at 15.5°.
THALLIUM THIOCYANATE T1SCN.
SOLUBILITY IN WATER AND IN AQUEOUS SALT SOLUTIONS.
(Bottger, 1903; Noyes, 1890; Noyes and Abbott, 1895.)
One liter sat. aq. solution contains 3.154 gms. T1SCN at 20°, 3.905 gms. at 25*
and 7.269 gms. at 39.75°.
Aq. Salt Solution.
Gms. Mols. per Liter.
SalT T1SCN.
Thallium BromateTlBrOa (excess) 39-75 0.01496 O.O22I
Gms. per Liter.
Thallium Nitrate T1NO3
«
Potassium Thiocyanate, KSCN
25
25
25
0.0227
0.0822
Salt. T1SCN.
4.966 5.793(N.&A.)
0.00852 6.04. 2.233(N.)
0.00406 21.88 . 1.064
0.0083 2.208 2.i76(N.)
721
THALLIUM VANADATES
THALLIUM VANADATES.
SOLUBILITY IN WATER.
Vanadate.
Tl. meta vanadate
" ortho vanadate
" pyro vanadate
" vanadate
Formula.
T1V03
(Carnelly, 1873; Liebig, 1860.)
Gms. Vanadate per 100 Gms. H2O.
At 15°.
0.087 C1*0
I
O.20 (14°)
0.107
THEBAINE (Para Morphine) Ci9H2iNO3.
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent.
92 Wt. % Alcohol
Ether
Aniline
Pyridine
Piperidine
Diethylamine
THEOBROMINE (Dimethyl Xanthine) C6H2(CH3)2N402.
SOLUBILITY IN SEVERAL SOLVENTS.
t°.
Gms. Thebaine per
100 Gms. Solvent.
25
O.I
10
0.71
20
30
20
9
20
2
2O
0.7
At i oo6.
0-21
1.74
0.26
°-29
Authority.
(Scholtz, 1912.)
Solvent.
Water
t°.
N4O2 per zoo Gms.
Solvent.
Authority.
18
0.0305
(Paul, 1901.)
15-20
0.059
(Squire & Caines, 1905.)
18
0.047
(Paul, 1901.)
18
0.083
"
18
I.78
it
18
4.56
"
15
3.69
(Brissemoret, 1898.)
21
0.045
(Squire & Caines, 1905.)
15-20
O.O2
"
15
0.005
(Wester & Bruins, 1914.)
15
O.OOS
"
b. pt.
0.021;
(Gockel, 1897.)
b..pt.
0.032
"
Aq. 0.25 n HC1
" i wHCl
" o.i wNaOH
" 0.25 n "
" i5.6percentNa3(PO4)2.Sol.
92.3 Wt. % Alcohol
90 Wt. % Alcohol
Dichlorethylene
Trichlorethylene
Carbon Tetrachloride
Ether
THIOPHENE MonoCARBONIC ACIDS a, ft and a C4H3SCOOH.
The solubility of the three isomers is given by Voerman (1907) as 0.57 gm. of
the a acid per 100 cc. sat. solution at 21°; 0.445 gm- of the 0 acid at 18°, and 0.75
gm. of the a acid at 17°. The solvent is not stated. Data for the solidification
points of mixtures of the a and /3 acid are also given. •
THEOPHYLLINE (Theocin) C6H2(CH3)2N4O2.H2O.
100 gms. H2O dissolve 0.52 gm. theophylline at 15-20°. (Squire & Caines, 1905.)
100 cc. 90 vol. % alcohol dissolve 1.25 gms. theophylline at 15-20°.
THORIUM EMANATIONS.
Data for the solubility of thorium emanations are given by Klaus (1905).
THORIUM ChloroACETATES.
SOLUBILITY IN WATER AT 25°. (Karl. 1310.)
Name of Salt. Formula. SS^SfjR
Basic Thorium Monochloroacetate (ClCH2COO)2Th(OH)2.H2O 0.0663
Basic Thorium Dichloroacetate (Cl2CHCOO)2Th(OH)2 0.0887
Basic Thorium Trichloroacetate (Cl3C.COO)2Th(OH)2 0.0091
THORIUM BORATE
722
THORIUM BORATE.
The precipitate which results when thorium nitrate is added to a solution of
borax is not a stable compound. Solubility determinations made by four suc-
cessive extractions of it at 18° with water, gave the following gms. of material
per 100 gms. H2O; 0.5366, 0.1250, 0.0611 and 0.0560. After the fourth ex-
traction, the residue then contained 10.14% B2O3 and after boiling 10 gms.
with 100 cc. of H2O for 6 hrs. and repeating this four times, it contained 9.63-
9.81% B2O3. (Karl, 1910.)
THORIUM HIPPURATE Th(C6H6.CO.CH2.NH.COO)4.
100 gms. H2O dissolve 0.0318 gm. of the salt at 25°.
(Karl, 1910.)
THORIUM OXALATE Th(C2O4)2.6H2O.
SOLUBILITY IN AQUEOUS SOLUTIONS OF AMMONIUM OXALATE AT 25°.
(Hauser and Wirth, igoga, 1912.)
Gm. Mols. per 1000 Gms.
Sat. Sol.
(NHOzCA.
Th(CA),.
0.00033
0.00005
0.00072
O.OOOI2
0.00120
O.OOO2O8
O.OOI53
0.00026
o.6oif
0.195
i.iSif
0.427
1.420}
0.540
i.48ot
0.563
Solid Phase.
Th(CA)2.6H20
[Th(C204]3(NH4)2.3H20
Normality
Vjms. J.n\j2
per
1000 Gms.
Sat. Sol.
0.01
0.040
O.IO
0.5*
2.203
7.660
10.63
0.5*
0.5*
0.5*
15.90
17.60
17-75
Solid Phase.
[Th,(CA>iKNHl)fr7HlO
* In these cases the greater part of the ammonium salt entered the solid phase complex and it was,
therefore, necessary to add additional ammonium oxalate until constant results were obtained.
t In these cases the solvent was saturated ammonium oxalate solutions containing an excess of the
crystals.
A thorium ammonium oxalate of the composition Th(C2O4.NH4)4.4H2O is
described by Brauner (1898). It is partially hydrolytically decomposed in
aqueous solution and a solubility determination made by analyzing the solution
from which the nearly pure salt began to crystallize, showed that 100 gms. H2O
contain 90.3 gms. Th(C2O4.NH4)4.4H2O and 9.3 gms. of (NH4)2C2O4 (= an addi-
tional \ mol. wt.)
SOLUBILITY OF THORIUM OXALATE IN AQUEOUS SOLUTIONS OF
HYDROCHLORIC ACID.
Solid Phase.
Results at 17°.
Results at 25°.
(Colani, 1913.)
(Hauser and Wirth, 1912.)
Gms. per 100 Gms.
Sat. Sol.
Cone, of
Aq. HC1 in
Gm. ThO2 per
1000 Gms. Sc
HC1. ThtCjOOj.
Per cent.
Sat. Sol.
o 0.0017
24.8
0 . 100 3Th(C
1.2 0.0035
37
3-450
3.6 0.0061
37-6
3-492
4.6 0.0094
8.4 0.017
13.1 0.028
16.2 0.038
19.8 0.064
Results at 50°.
(Colani, 1913.)
Gms. per 100 Gms.
Sat. Sol.
HC1.
0
Th(C204)2.
0.0017
4.1
8-4
0.010
0.028
12.4
16.1
18
19.9
21.6
0.057
0.103
0.134
0.169
0.232
Data are also given for the solubility of thorium oxalate in aqueous solutions
of mixtures of hydrochloric and oxalic acids at the above temperatures.
723
THORIUM OXALATE
SOLUBILITY OF THORIUM CHLOROOXALATE, 3Th(C2O4)2ThCl4.2H2O, IN AQUEOUS
HYDROCHLORIC ACID.
(Colani, 1913.)
Cms, per 100 Gms. Sat. Sol.
12
15
12
15
12
IS
' HC1.
Th4(c2o4)ci4:
23
26.3
O.I2
0.17
29.9
32.5
0.27
0.48
33-1
0-53
35
1.03
50
50
50
50
50
50
Cms, per 100 Gms. Sat. Sol.
HCL '
21.2
23
26.8
29.8
32.3
34-6
0.29
0.34
0.46
0.75
1.51
2.59
Results are also given showing the effect of oxalic acid upon the solubility of
the above salt in aqueous hydrochloric acid.
SOLUBILITY OF THORIUM OXALATE IN AQUEOUS OXALIC ACID SOLUTIONS.
Results at 25°.
(Hauser and Wirth, 1912.)
Normality of
Aq.H2CA.
Gm. ThO2 per
1000 Gms. Sat.Sol.
<, ,. , p,
Sohd Phase.
Results at 50°.
(Colani, 1913.)
Gms. per 100 Gms. Sat. Sol.
H2C2Q4.
I 0.0015 Th(C2O4)2.6H2O 1.7
Sat. Solution 0.0030 " +H2c2o4.2H2o 9.3
03
SOLUBILITY OF THORIUM OXALATE IN AQUEOUS SOLUTIONS OF SULFURIC
ACID AT 25°.
(Hauser and Wirth, igoga, 1912; Wirth,
Th.
0.0002
o.ooi
0.003
Nonnalityof
Aq.H2S04.
0.25
0.5
i
2.1
3.2
Sat. Sol.
0.07
0.14
0.26
0.418
0.71
Solid Phase.
Th(C2O4)2.6H2O
4.32
4-9
6.175
6.885
8.45
Sat. Sol.
1. 10
1.32
1.513
1.794
2.473
Solid Phase.
Th(CjO4)2.6H2O
THORIUM PICRATE Th(C6H2N3O7)4.ioH2O.
100 gms. H2O dissolve 0.3052 gm. of the salt at 25°.
THORIUM SELENATE Th(SeO4)2.9H2O.
100 gms. H2O dissolve 0.498 gm. Th(SeO4)4 at o° and 1.972 gms. at 100°.
THORIUM SULFATE Th(SO4)2.
SOLUBILITY IN WATER.
(Roozeboom, 1890; Demarcay, 1883.)
(Karl, 1910.)
(Cleve, 1885.)
Gms. Th(SO4)2
Per Solid
-o Gms. Th(SO4)2 per
100 Gms. H2O.
Solid
Phase.
'
100 Gms.
H20. ' Phase.
O
0
•74<R)
0
.88(D) Th(S04)2.9H20
O
i
•5o(R)
Th(SO4)2.6H2O
10
0
.98
I
.02
15
i
•63
"
20
X
•38
I
•25
30
2
•45
44
30
I
•995
I
.85
45
3
•85
44
40
2
.998
2
.83
60
6
.64
"
5°
5
•22(51°)
4
.86
17
9
.41 (D)
ThCSOJj^HjO
55
6
.76
6
•5±
40
4. 04 (R) 4 -5 (35° E>)
o
i
.0
Th(SC>4)2.8Ha
50
2-54
1.94
(55")
44
15
i
•38
60
1-63
"
25
X
•85
44
70
1.09
1.32
(75°)
•
44
3
•71
•
95
0.71
n
Additional results for the .8H2O and the .9H2O salt, in fair agreement with the
above, are given by Wyrouboff (1901).
THORIUM SULFATE
724
SOLUBILITY OF THORIUM SULFATE IN
AQUEOUS SOLUTIONS OF:
Ammonium Sulfate at 16°.
Lithium Sulfate at 25°.
(Barre, igii.)
(Barre, 1912.)
Gms. per 100 Gms. H2O.
Solid Phase.
Gms. per 100 Gms. H2O.
(NH4)2SO4. Th(SO4)2.
Li2S04. Th(S04)2:
2.13 3.361
TKSO^.gl^O
o 1.722
4.80 5.269
"
2-57 4-13
10.02 8.947
"
4-93 6.20
•16.56 I3-330
" +1.1.4
6.98 7-95
28 10.359
1.1.4
9.23 9.68
35.20 9.821
" +1.2.2
11.13 11.05
45.14 6.592
1.2.2-
13.18 12.54
49-05 5-750
''
16.12 14-52
52.88 4.583
1-3-3
2O.49 l6.Q2
69.74 1.653
"
25.18 18.87
1.1.4 = Th(S04)2.(NH4)2S04.4H20; 1.2.2 =
Th(S04)2.2(NH4)2S04.2H20; 1.3.3
Th(S04)2.3(NH4)2S04.3H20.
SOLUBILITY OF THORIUM
Results at 16°.
Gms. per 100 Gms. H2O.
K2S04.
Th(SOJ2.
0
i-39
0.424
1.667
.004
2.193
•152
3-i9i
.224
2.514
.283
2.222
.348
1.706
-378
I-637
.487
0.870
.844
0.370
3.092
0.070
4- 050
O.O27
4.825
0.003
SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM
SULFATE.
(Barre, 1911.)
Results at 75°.
Solid Phase.
Gms. per 100 Gms. H2O.
Th(S04)2.K2S04.4H20
K2SO4.
O
0.865
1.167
0.9248
i-i37
I-I73
1 .172
I .121
1 .270
1.296
1.852
0.907
0-495
0.297
3-«7
4-659
5-348
O.2OI
0.256
0.170
5-932
0.123
7.177
9.706
0.031
O.O22
Th(S04)2.3^K2S04
SOLUBILITY OF THORIUM SULFATE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC
ACID AND OF NITRIC ACID AT 30°.
(Koppel and Holtkamp, 1910.)
In Aq. Hydrochloric Acid.
Wt. % HC1
in Solvent.
Gms. Th(SO4)'
per too Gms.
Sat. Sol.
0
2.15
4-55
3-541
6-95
3-431
12.14
2.811
15.71
2.360
18.33
2.199
20
2.IIO
20
2.I4I
23-9
1.277
Solid Phase.
In Aq. Nitric Acid.
Solid Phase.
Wt. % HN03
in Solvent.
oms. iiivov.
per zoo Gn
Sat. Sol.
0
5-17
2-15
3-68
IO.O4
16.68
4.20
4.84
21.99
28.33
28.51
4-47
3-88
33-17
38.82
3-34
2.51
725
THORIUM SULFATE
SOLUBILITY OF THORIUM SULFATE IN AQUEOUS SOLUTIONS OF:
Sodium Sulfate at 16°.
(Barre, 1910, 1911.)
Gms. per 100 Gms. H20.
Sulfuric Acid at 25°.
(Barre, 1912.)
Gms. per 100 Gms. H2O.
Na2S04.
1.094
1.960
2.98
4.II
5-79
9-35
12.24
15-36
1 . 7432 ThtSO^.NajSCVGHjO
2.387
3-962
3-375
2.136
1-379
1.169
i . 048
H2S04.
O
1.072
I.94I
2.821
3.843
5.212
8.055
10.105
1.722
I.9I9
2.OI7
2.060
2.o6l
2.035
1.863
I.7O2
SOLUBILITY OF THORIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC ACID
Results at 25°.
(Wirth, 1912.)
Results at 20° and at the b.-pt.
(Koppel and Holtkamp 1910.)
Normality Gms. Th(SO4)2
Wt. %
Gms. Th(SO4)2
of
per 100 Gms. Solid Phase.
t°. H2SO4 in
per loo Gms.
Solid Phase.
Aq. H2S04.
Sat. Sol.
Solvent.
Sat. Sol.
O
1 . 593 Th(S04)2.9H20
20 5
1.722
Th(SO4)2.8HJO
I.I
1.831
20 15
0.9752
"
2.l6
1.488
20 25
0.3838
"
4-32
0.8751
2O 40
O.OIO3
ThtSO^^HjO
6.68
0.4312
b. pt. 5
0.7407
TMSOJj.SHjO
9.68
0.1045 Th(SO4)».8HaO
IO
0.4808
"
10.89
0.0636
IS
0.3882
"
15.15
0.0308 Th(SO4)i.4HjO
Results at 30°.
(Koppel and Holtkamp, 1910.)
Wt. % H2SO4
in Solvent.
Gms. ThCSOt), per Solid Phase Wt. % H2SO4 Gms. ThCSO^j p
100 Gms. Sat. Sol. in Solvent. looGms. Sat. So
fr Solid Phase.
0
2.152 Th(SO4)t.8
H2O 15.03
1.484
TMSO^.SHjO
0.466
2.055
23.64
0.7196
"
0.72
2.085
32.68
0.3364
"
1.468
2.267
37-80
0.077
Th(S04)*.4HtO
2.983
2.3H
43.28
0.0213
"
4.38
2.367
45.69
0.0047
"
4-97
2.323
74
o.i 208
«
9-95
1 . 961
80.5
0
"
THORIUM m Nitrobenzene SULFONATE Th(C6H4.NO2.SO3)4.7H2O.
100 gms. H2O dissolve 61 gms. of the anhydrous salt at 15°. (Holmberg, 1907.)
THULIUM OXALATE Tma(C2O4)3.9H2O(?.ioH2O).
100 cc. aq. 20% methyl amine oxalate dissolve approx. 4.082 gms. thulium oxalate.
100 cc. aq. 20% ethylamine oxalate dissolve approx. 5.728 gms. thulium oxalate.
loo cc. aq. 20% triethylamine oxalate dissolve approx. 1 .340 gms. thulium oxalate.
(Grant and James, 1917.)
THULIUM Bromonitrobenzene SULFONATE Tm(C6H3Br.NO2.SO3, 1.4.2)3.-
I2H2O.
100 gms. sat. solution in water contain 6.379 Sms. of the anhydrous salt at 25°.
(Katz and James, 1913.)
THYMOL (3 Methyl 6 Isopropyl Phenol) C3H7.C6H3.OH.CH3.
SOLUBILITY IN WATER. (Seidell, 1912.)
f o Gms. Thymol per f 0 Gms. Thymol per
zoo Gms. Sat. Sol. 100 Gms. Sat. Sol.
10 0.067 25 0.0995 37 0.132
15 0.077 3° 0.112 40 0.141
20 0.088 35
O.II2
O.I26
Gms. Thymol per
100 Gms. Sat. Sol.
THYMOL 726
SOLUBILITY OF THYMOL IN AQUEOUS HYDROCHLORIC ACID. (Seideii, 1912.)
Normality of Gm. Thymol per 100 cc. Sat. Sol, at:
Aq.HCl.
o
O.I
O.5
I
2.5
5
100 cc. 90 vol. per cent alcohol dissolve about 300 gms. of thymol at I5°-2O°.
(Squire and Caines, 1905.)
SOLUBILITY OF THYMOL IN SEVERAL OILS. (Seideii, 1912.)
Gms. Thymol per 100 Gms. of:
25°.
37.2°.
0.0995
O.O968 (^26 = I.OO2)
O . 0884 (^25 = I «OOg)
O.O8O2 (<*2S = I.Ol8)
0.132
0.129
O.I2I
O.II2
0.0612 (1*25 = 1.043)
0.0935
0.0445
O.O772
t°.
Olive
Peanut
Cod Liver
Liquid
Castor
Cottonseed
Linseed
Oil.
Oil.
Oil.
Petrolatum.
Oil.
Oil.
Oil.
10
46.2
73
50
3-i
8l.2
56.2
62.3
IS
50-1
73-8
52
3-95
Q0.2
64
63-1
20
56.2
74.6
55-5
5-6
101 .5
74.2
65.1
25
66.9
76.4
63.1
9.78
Il6.5
89.4
69
30
84.5
83.2
77
16.3
137 '
II3-7
78.3
35
III
106.7
102
25-5
165
146.5
100
37
124-3
130.5
II6.5
29.9
180
166.5
II6.5
40
I5I-9
212.5
150
38-9
213
217-5
152
The specific gravities of the above saturated solutions and of solutions of
lower concentrations of thymol in the several oils are also given.
DISTRIBUTION OF THYMOL BETWEEN WATER AND OILS AT 25° AND AT 37°.
(Seideii, 1912.)
Water + Olive Oil. Water + Cod Liver Oil. Water + Peanut Oil.
Gms. Thymol per TOO cc. Gms. Thymol per 100 cc. Gms. Thymol per TOO cc.
*"• ' OH i£o ' — • ' oii 5^5 ' — • ' oii H^T" -r-
Layer (c0). Layer (cj. Cw Layer (c0) Layer (cw). Cv> Layer (c0). Layer (c«,).
25 0.1014 44-95 443 0.1079 49 454 0.1077 46.48 431
25 0.0848 36.. 34 428 0.0816 32.58 400 0.0786 32.45 413
25 0.0349 16.26 465 0.0371 16.18 436 0.0395 16.16 409
25 0.0106 4.54 430 0.0127 4-57 359 o.oo88(?) 4.63 523
37 0.1087 46.35 427 0.1099 43-8i 399
37 0.0807 33-48 415 0.0862 32.90 380
37 0.0381 16.24 426 0.0574 22.51 392
37 0.0122 4.61 378 0.0250 8.86 357
Freezing-point data for mixtures of thymol and sulfuric acid are given by
Kendall and Carpenter (1914).
Results for thymol + bromotoluene are given by Paterno and Ampola (1897).
TIN Sn.
DISTRIBUTION OF TIN BETWEEN AQUEOUS HYDROCHLORIC ACID AND ETHER AT
ROOM TEMPERATURE. (Mylius, 1911.)
When i gm. of tin as the chloride, SnCl4, is dissolved in 100 cc. of aqueous
hydrochloric acid and shaken with 100 cc. of ether, the following per cents of the
metal enter the ethereal layers. With 20% HC1, 17 per cent; with 15% HC1,
28 per cent; with 10% HC1, 23 per cent; with 5% HC1, 10 per cent and with
i% HC1, 0.8 per cent of the tin.
727 TIN CHLORIDE
TIN CHLORIDE (Stannous) SnCl*.
100 gms. H2O dissolve 83.9 gms. SnCl2 at o° and 269.8 gms. at 15°. Sp. Gr.
of Solutions 1.532 and 1.827 respectively. (Engel, 1889; Michel and Krafft, 1851.)
SOLUBILITY OF STANNOUS CHLORIDE IN AQUEOUS SOLUTIONS OF
HYDROCHLORIDE ACID AT o°.
(Engel.)
Milligram
Mols. per 10 cc.
Sp. Gr.
Grams per 100 cc.
Solution.
of
Solution.
HC1.
iSnCl*.
Solution.
HC1.
SnClj.
0
74-0
• 1-532
o.o
70.26
6.6
66.7
1.489
2.405
63-33
13-54
63-7S
1.472
4-935
60.52
24.8
68.4
1.524
9.04
64.95
34-9
8l.2
I .625
12.72
77.11
40-0
94.2
1.724
14.58
89.45
44-o
117.6
1.883
16.04
111-7
49-4
147.6
2.II4
18.01
I38.6
66.0
156.4
2.190
24.05
148.5
78.0
157-0
2.199
28.43
149.0
100 gms. acetone dissolve 55.6 gms. SnCl2 at 18°. (dip =
1.6.) (Naumann,
1904.)
100 gms. ether
100 gms. ethyl
dissolve 11.4 gms. SnCl2.2H
acetate dissolve 31.2 gms.
2O at o°-35.5°.
SnCl2.2H2O at
-2°, 35-53 gms. at
+22° and 73-44 gms. at 82°. (von Laszynski, 1894.)
100 gms. ethyl acetate dissolve 4.46 gms. SnCl2 at 18°. dip of the sat. solution
= 0.9215. (Naumann, 1910.)
ioo gms. 95 per cent formic acid dissolve 4.1 gms. SnCl2 at 19°. (Aschan, 1913.)
Freezing-point data for mixtures of SnCl2 + ZnCl2 are given by Herrmann
(1911).
TIN CHLORIDE (Stannic) SnCl4.
DISTRIBUTION OF STANNIC CHLORIDE BETWEEN WATER AND XYLENE.
(Smirnoff, 1907.)
Very concentrated aqueous stannic chloride solutions were agitated with
xylene at various temperatures and the amount of SnCl4f in terms of Cl, which
entered the xylene layer was determined. The amount of Sn and Cl in the
xylene was found to correspond to SnCl4.
Results for Xylene + SnCl4.5H20. Results for Xylene + SnCl4.4H2O.
Gms. Cl per ioo Gms.
^
Gms. Cl per ioo Gms.
c
t°.
Aq.
Layer, c.
Xylene
Layer, c'.
c'
r.
Aq.
Layer, c.
Xylene
Layer, c'.
66
40.35
0.08
504.4
66
41.9
0.92
45-3
80
39-95
0.18
228.5
80
41.91
1.56
27
97-5
40.24
0-33
122. I
IOO
41.85
2.52
!6.7
in
40.27
0.68
59-3
III
41.68
3-23
12.9
Per cent Cl in SnCl4.sH2O = 40.38. Per cent Cl in SnCl4.4H2O = 42.37.
Results for Xylene + SnCl4.3H2O.
Gms. Cl per too Gms.
t°« Aq. Xylene ~i'
Layer, c. Layer, c'.
80 43.2 . 9.93 4.4
94 42.54 9.32 4.6
ioo 42.64 10.56 4.1
in 42.31 10.03 4-2
Per cent Cl in SnCl4.3H2O = 45.12.
TIN HYDROXIDE 728
TIN HYDROXIDE (Stannous) Sn(OH)2.
One liter of the saturated solution in water contains 0.0000135 gm. mols.
Sn(QH)2 at 25°. (Goldschmidt and Eckhardt, 1906.)
SOLUBILITY OF STANNOUS HYDROXIDE IN AQUEOUS SODIUM HYDROXIDE
SOLUTIONS AT 25°.
(Goldschmidt and Eckhardt, 1906.)
The authors desired to ascertain whether the mono, NaHSnO2, or the disodium
salt, Na2SnC>2, predominates in alkaline tin hydroxide solutions. Given amounts
of carefully prepared tin chloride, made from tin and HC1, and sodium hydroxide
solutions were mixed in vessels containing hydrogen. The mixtures were shaken
at 25° and the clear supernatant solutions in contact with the precipitated
Sn(OH)2, analyzed.
Gm. Mols. per Liter. Gm. Mols. per Liter.
Total Na.
NaHSn02.
NaOH.
Total Na.
NaHSnO2.
NaOH.
0.00451
0.0009845
0.003525
0.02250
0.00838
O.OI4I2
0.00(58o
0.002l8
0.00462
0.02788
0.01038
0.01755
0.01149
0.003495
0.007995
0.02940
0.00874
O.O2066
0.02143
0.006935
0.014495
O.03OI2
0.00865
0.02147
0.02143
O.00660
0.01483
0.03036
O.OIO82
0.01954
0.02186
0.00628
0-015575
0.03044
0.009405
0.021035
SOLUBILITY IN AQUEOUS SODIUM HYDROXIDE SOLUTIONS. MOIST TIN
HYDROXIDE USED. ORDINARY TEMPERATURE.
(Rubenbauer, 1902.)
Gms. per 20 cc. Mol.
Solution. Dilution of the
Gms. per 20 cc. Mol.
Solution. Dilution of the
Na.
o . 2480
0.3680
0.6394
Sn.
0.1904
0.2614'
0.4304
NaOH.
1.86
i-*5
0.72
Na.
0.8326
0.9661
2.1234
Sn/
0.5560
0.7849
1.8934
NaOH.
o-55
'0.48
0.23
TIN IODIDE (Stannous) SnI2.
SOLUBILITY IN WATER AND IN AQUEOUS HYDRIODIC ACID.
(Young, 1897.)
t*. Gms. Snla per 100 Gms. Aqueous HI Solutions of:
'
o^=H20.
5-83%.
9-60%.
15-2%.
20.44%.
24-8%.
30.4%.
36.82%.
2O
0.98 '
O-2O
0.23
0.6O
1.81
4-20
10.86
25 -31
30
1.16
0.23
0.23
0.64
1.81
4.06
10.28
23.46
40
i .40
o-33
0.28
0.71
1.90
4-12
10. 06
23-15
5°
i .69
0.46
0.38
0.82
2 .12
4-34
10.35
23.76
6o
2.07
0.66
o-55
I .11
2.51
4.78
11.03
24.64
70
2.48
0.91
0.80
I .37
2.92
5-43
11.97
25.72
80
2-95
1.23
1.13
1.83
3-70
6.38
I3-30
27.23
9o
1.65
1.52
2.4O
4.58
7.82
I5-52
29.84
100
4-03
2.23
2.04
3-63
5-82
9.60
34-os
TIN; IODIDE (Stannic) SnI4.
SOLUBILITY IN ORGANIC SOLVENTS.
(McDermott, 1911.)
+° Sp. Gr. Gms. SnL, per
Sat. Sol. 100 Gms. Sat. Sol.
Carbon Tetrachloride 22.4 1.59 5.25
50 1.63 12.50
Chloroform 28 1.50 8.21
Benzene 20.2 0.95 12.65
729 TIN IODIDE
SOLUBILITY OF STANNIC IODIDE IN CARBON DISULFIDE.
(Sneider, 1866; Arctowski, iSgs-'gG.)
— ii4°.S. —94°. ^-89°. —84°. —58°. Ord. temp.
Cms. Snl4 per 100 Gms.
Solution 9.41 10.65 9-68 10.22 16.27 59.2(8)
100 gms. methylene iodide, CH2I2, dissolve 22.9 gms. SnI4 at 10°. Sp. Gr. of
solution = 3.481. (Retgers, 1893-)
TIN OXALATE (Stannous) Sn(COO)2.
100 gms. 95 per cent formic acid dissolve 0.16 gm. Sn(COO)2 at 19°. (Aschan, 1913.)
TIN TetraPHENYL (Stannic) Sn(C6H6)4.
Freezing-point data for Sn(C6H6)4 + Si(C6H6)4 are given by Pascal (1912).
TIN SULFATE (Stannous) SnSO4.
100 gms. H2O dissolve 18.8 gms. SnSO4 at 19° and 18.1 gms. at 100°. (Marignac.)
TOLUENE C6H6CH3.
SOLUBILITY IN SULFUR.
Figures read from curve, synthetic method used, see Note, page 16. (Alexejew, 1886.)
Gms. CeHsCHg per 100 Gms. Gms. CpHsCHa per 100 Gms
* °- '~S Toluene * °* /~S Toluene
Layer. Layer. Layer. Layer.
ioo 3 73 150 12.5 59
no 4 71 160 16 53
120 5 68 170 22 47
130 7 66 175 25 43
140 9.5 63 178 crit. temp. 34
NitroTOLUENE o C6H4.CH3.NO2.
RECIPROCAL SOLUBILITY OF o NITROTOLUENE AND WATER.
(Campetti and Delgrosso, 1913.)
The original results were plotted and the following figures read from the
curve.
Gms. o Nitrotoluene per ioo Gms. Gms. o Nitrotoluene per ioo Gms.
t°. H2O Rich Nitrotoluene *"• H2O Rich Nitrotoluene'
Layer. Rich Layer. Layer. Rich Layer.
150 i 98 245 13 81
175 1.5 96 250 16 78
200 3 93 255 20 72
225 6.5 89 260 29 63
240 10.5 84 263. 5 crit. t. 43
ioo gms. 95 per cent formic acid dissolve 13.25 gms. p CeH4.CH3.NO2 at 20.8°.
(Aschan, 1913.)
TrinitroTOLUENE 2,4,6 C6H2.CH3(NO2)3.
ioo gms. H2O dissolve 0.021 gm. C6H2.CH3(NO2)3 at 15° and 0.164 Sm- at IOO°'
ioo gms. alcohol dissolve 1.6 gms. C6H2CH3(NO2)3 at 22° and 10 gms. at 58°.
(Capisarow, 1915-)
TOLUENE SULFONAMINES o, m and p.
SOLUBILITY OF EACH IN WATER AT 25°. (Holleman and Caland (1911-)
Compound. Gins. Cgmp'djjer Liter
Amine of o Toluene Sulfonic Acid i .624
" " m " " 7.812
" " p " " " 3-156
TOLUENE 730
FREEZING-POINT DATA (Solubility, see footnote, p. i), FOR MIXTURES OF SUB-
STITUTED TOLUENES AND OTHER COMPOUNDS.
Mixture. Authority.
o Bromotoluene + p Bromotoluene (van der Laan, 1907.)
Bromotoluene + p Xylene fPaterno and Ampola, 1897.)
+ Veratrol
-f- Tribenzylamine " "
p Nitrotoluene + « Ortho Nitrotoluene (Holleman, 1914.)
+ 2, 4 Dinitrotoluene (Giua, 1914, 1915.)
+ 2, 6 (Giua, 1915.)
+ 2,4,6
+ m Nitrotoluene (Holleman and van den Arend, 1909.)
+ Urethan (Mascarelli, 1908, 1909.)
2, 4 Dinitrotoluene + 2, 6 Dinitrotoluene (Giua, 1914, 1915.)
+ 2, 4, 6 Trinitrotoluene (Giua, 1915.)
2, 6 + (Giua, 1914, 1915.)
a Trinitrotoluene -f- p Amino Acetophenone (Giua, 1916.)
+ 7 Trinitrotoluene (Giua, 1915.)
o Toluene Sulfochloride + p Toluene Sulfochloride (Holleman and Caland, 1911.)
Binary Mixtures of Isomeric Tribromotoluenes (Jaeger, 1904.)
" Chloronitrotoluenes (Wjbaut, I9i3; Holleman and van den
Arend, 1909.)
TOLUIC ACIDS (Monomethyl Benzole Acids) CH3.C6H4COOH.
SOLUBILITY IN WATER AT 25°.
(Paul, 1894.)
Add CH3.C6H4.COOH per Liter Solution.
Grams. Millimols.
Meta Toluic Acid 0.9801 7.207
Ortho Toluic Acid i . 1816 8 . 683
Para Toluic Acid 0.3454 2.540
One liter sat. solution in water contains 0.42 gram p toluic acid at 25°. One liter
sat. solution in i n aq. sodium p toluate contains 0.735 gm- P toluic acid at 25°.
(Sidgwick, 1910.)
SOLUBILITY OF TOLUIC ACIDS (EACH SEPARATELY) IN WATER AT VARIOUS
TEMPERATURES.
(Sidgwick, Spurrell and Davies, 1915.)
The determinations were made by the synthetic method, see p. 16; melting-
point of o toluic acid = 102.4°, of m acid = 110.5° and of p acid = 176.8°. The
triple point (solid phase present) for the o acid, is at 93.5° and the concentration
of acid in the two layers is 2.5 and 91.2 gms. respectively per 100 gms. sat. solu-
tion. The tr. pt. for the m acid is at 91.8° and concentrations are 1.6 and 90.5;
the tr.-pt. for the p acid is at 142° and concentrations, 5 and 74.
Gms. per 100 Gms. Sat. Sol.
Gms. per 100 Gms. Sat. Sol.
*°- o Toluic
m Toluic
P Toluic * •
o Toluic
m Toluic
* Toluic
Acid.
Acid.
Acid.
Acid.
Acid.
Acid.
80
2
•03*
1.16*
140
9-
25
5-77
4.30*
90
2
•42*
i-54
. . .
ISO
13-
7
8.40
9-33
100
2
•97
1.98
I
.16*
159
. i crit t.
. .
.
. . .
00
no
3
•7i
2.52
I
.36*
1 60
30
19.4
120
5
.10
3-24
1
•75*
161
. i crit. t.
00
130
6
•93
4-30
2
.50*
162
. 2 crit. t.
00
* Indicates that a solid phase is present.
Additional data for the solubility of the above compounds in water, determined
by the synthetic method, are given by Flaschner and Rankin (1910).
731 TOLUIC ACIDS
RATIO OF THE SOLUBILITIES OF TOLUIC ACIDS (SEPARATELY DETERMINED)
IN WATER AND IN OLIVE OIL AT 25°.
(Boeseken and Waterman, 1911, 1912.)
The solubilities of each acid in water and in olive oil was separately determined
and the ratio considered to correspond to the distribution coefficients in each
case. The concentrations of the dissolved acids are not given.
n t. , Solubility m Olive Oil
Acid. Ratio of 0 . .... — 1—7= •
Solubility m Water
o Toluic Acid 40 . 5
m " " 21 *
p 39.5
100 gms. 95% formic acid dissolve 2.99 gms. o toluic acid at 20.8°. (Aschan, 1913.)
Freezing-point data for mixtures of o, m, p and a toluic acids (each separ-
ately) and sulfuric acid are given by Kendall and Carpenter (1914). Results for
mixtures of o, m and a acids and picric acid are given by Kendall (1916).
TOLUIDINE C6H4CH3.NH2.
SOLUBILITY IN WATER.
(Vaubel, 1895; Lowenherz, 1898.)
Gms. Gms.
to CeHiCHa-NHa Solid to CeRkCHjjNHa Solid
per 1000 Phase. per 1000 Phase.
Gms. H2O. Gms. H2O.
2O l6.26 Liquid ortho T. 2O-8 7.39 Para T.
20 0.15 Ortho T. 26.7 9.50 "
20 6.54 ParaTc 31.7 11.42 "
One liter sat. solution in water contains 15 gms. o toluidine at 25°.
One liter sat. solution in i n aq. o toluidine hydrochloride, contains 30 gms.
o toluidine at 25°. (Sidgwick, 1910.)
The following results for p toluidine, differing considerably from the above,
are given by Walker (1890).
t°. 22° 30° 36.7° 44° 57-5° 69°
Gms. p Toluidine per 100 Gms.
Sat. Sol. in Water 19.6 26.9 35.4 44.5 51.4 58.9
SOLUBILITY OF PARA TOLUIDINE IN ETHYL ALCOHOL.
(Interpolated from original results of Speyers, 1902.)
Wt. Mols. per Gms. per Wt. Mols. per Gms. per
t*. of i cc. 100 Mols. too Gms. t°. of i cc. 100 Mols. 100 Gms.
Solution. C2H5OH. C2H6OH. Solution. C2H6OH.
O 0.8885 20.72 48.1 20 0.9265 47-0 IIO.O
5 0.8982 26.0 60.0 25 0.9360 56.0 132.0
10 0.9080 32.0 74 -o 30 0.9460 66. o 156.0
15 0.9180 38.6 90.0
ioo gms. pyridine dissolve 126 gms, p toluidine at 2O°-25°. (Dehn, 1917.)
100 gms. aq. 50% pyridine dissolve 96.1 gms. p toluidine at 2O°-25°. "
DISTRIBUTION OF PARA TOLUIDINE BETWEEN WATER AND CARBON
TETRACHLORIDE.
(Vaubel, 1903.)
Gm^Toluidim Votaes of Solvent, Cms. C.H/CH.)NH. » in:
Used- H2O Layer. CCU Layer.
i 200 cc. H2O+ioo cc. CCU 0.1406 0.8594
i 200 cc. H20-J-200 cc. CCU 0.0666 0.9334
TOLUIDINE 732
DISTRIBUTION OF o, m AND p TOLUIDINE BETWEEN WATER AND
BENZENE AT 25°.
(Farmer and Warth, 1904.)
Base. Dist.-Coef.^°nc-in^.
Cone, in H2O
o Toluidine 13.4
m " 19.1
P '4-1
Aceto TOLUIDINE p CH3C6H4NH.C2H3O.
SOLUBILITY IN MIXTURES OF ALCOHOL AND WATER AT 25°.
(Holleman and Antusch, 1894.)
Vol ^ Gms' P61" SP' Gr' Vol % Gms- Per SP- Gr°
AI YS ioo Gms. of Ai u i ioo Gms. of
Alcohol. Solvent> Solutions. AlcohoL Solvent. Solutions.
ioo 10.18 0.8074 50 1.92 0.9306
95 10.79 0.8276 45 1.41 0.9380
90 10.62 0.8440 40 0.96 0.9460
85 9.62 0.8576 35 0.66 0.9544
80 8.43 0.8685 25 0.31 0.9668
75 7.04 0.8803 20 0.23 0.9725
70 5-8i 0.8904 15 0.16 0.9780
65 4.39 0.9021 5 0.13 0.9903
60 3.59 0.9115 o 0.12 0.9979
55 2.69 0.9207
See remarks under a acetnaphthalide, p. 13.
TRIPHENYLAMINE, TRIPHENYLPHOSPHINE, etc.
F.-pt. data are given by Pascal (1912) for the following mixtures:
Triphenylamine + Triphenylarsine Triphenylarsine + Triphenyl Stibene
Triphenylamine + Triphenylphosphine Triphenylarsine + Triphenylbismuthine
Triphenylarsine -j- Triphenylphosphine Triphenylphosphine -f-
aand/S TRITHIOACET ALDEHYDE, (CH3CHS)3.
a. and 0 TRITHIOBENZALDEHYDE, (C6H6CHS)3.
SOLUBILITY OF EACH (DETERMINED SEPARATELY) IN SEVERAL SOLVENTS
AT 25°.
(Suyver, 1905.)
Gms. per ioo Gms. Solvent.
Solvent. , * v
«(CH3CHS)3. /3(CH3CHS)3. « (C6HBCHS)3. ft (C6H5CHS)3.
Ether 15-58 13-67 1.09 0.37
Ethyl Alcohol 3 . 86 3.97 o . 20 o . 04
Methyl Alcohol 4 . 04 3 . 89 0.17 o . 04
Acetone 20.96 18.31 2.45 1.12
Chloroform 57-59 51-22 ii.n 0.20
Carbon Bisulfide 25.50 20.75 5-8i 0-22
Benzene 36.40 26.98 6.08 0.014
Ethyl acetate *7-52 15-48 2.05 0.93
Data for the solidification points of mixtures of a and £ trithioacetaldehyde
are also given. Similar data for mixtures of a and /? trithiobenzaldehyde could
not be determined on account of decomposition with production of resins.
TROPIC ACID (« Phenylhydracrylic Acid) i and /, C6H6.CH(CH2OH)COOH.
ioo gms. sat. solution in H2O contain 1.975 Sms- °l tne * acjd at 20°. ) (Schlossberg.
ioo gms. sat. solution in HaO contain 2.408 gms. of the I acid at 20°. f 1900.)
733 TURPENTINE
TURPENTINE OIL
SOLUBILITY IN ETHYL ALCOHOL.
(Vezes and Mouline, 1904, 1905-06.)
Spirit of turpentine and absolute alcohol are miscible in all proportions and the
mixture may be cooled to a very low temperature without ceasing to be homo-
geneous. In the case of alcohol containing a small amount of water, the mixture,
which is uniform at ordinary temperature, separates into two layers when cooled.
The following data were obtained for mixtures of 98 vol. % alcohol ( = 0.968 gm.
C2HsOH per I gm. aq. alcohol) and spirits of turpentine and for mixtures of 95
vol. % alcohol ( = 0.924 gm. C2H5OH per I gm. aq. alcohol) and spirits of tur-
pentine.
Results for 98 Vol. % Alcohol. Results for 95 Vol. % Alcohol.
Cms.' 98 Vol. ,o . Cms. 98 Vol. , 0 . * Cms. 95 Vol. f „ _f Cms.
. 95
»
Mixture.
Mixture.
Mixture.
uon.
Mixture.
-35-6
2.7
— 20.9
32-9
+ 20.7
2.4
29.6
48.3
-23
4.8
— 26.1
42.6
42.2
3-4
23-9
52.8
— 2O-9
9-5
-30
48.2
" 53
7.2
16-3
61.4
-i8.i
13.2
-45-3
58
IO.2
-15-5
76.6
-17.8
16
-79.2
71.9
44
20.3
-24
81.1
-18.8
24.4
37-2
30.6
-63
87.1
Data in regard to the sample of spirits of turpentine which was used, are not
given.
URANYL Potassium BUTYRATE
The double salt is decomposed by water at ordinary temperatures and the solu-
tion gets richer in uranyl butyrate. The solubility at 29.4° in water containing
KC4H7O2 is 2.10 gms. UCMC^C^) + 0.38 gm. KC^H-jOz per 100 gms. solution.
The atomic relation being 1 : 0.64. (Rimbach, 1904.)
URANYL Ammonium CARBONATE
SOLUBILITY IN WATER.
(Giolitti and Vecchiarelli, 1905.)
A large excess of the double carbonate was agitated with water at constant
temperature and the clear saturated solutions analyzed.
Gms. per 100 Gms. Sat. Sol. Mol. Ratio.
U! CO2. NH3. /U I COT : NH3. "
18.6 2.71 1.54 0.795 I 3-o8 4.10
36.5 3.09 2.29 1.188 i 4.01 5.35
48.3 3.03 2.71 1.35 i 4-95 6.35
62 ... 3-*7 i -62 ... ...
87-3 3-95 3-96 2.027 i 5.42 7.15
Theoretical molecular ratio for UO2CO3.2(NH4)2CO3 = 1:3:4.
Thus at the lower temperature, the composition of the dissolved salt is very
near the ratio corresponding to the formula.
The author calculates that 6.04 gms. of UO-jCOs^CNH^COs are contained in
loo gms. of the sat. solution at 18.6° (a recalculation from the U value, 2.71, in-
dicates that this figure should be 5.26 gms.).
URANYL CHLORIDE UO2C12.3H2O.
IOO gms. H2O dissolve 320 gms. UO2C12 at 18°. (Mylius and Dietz, 1901.)
URANYL CHLORIDES
734
SOLUBILITY OF URANYL AMMONIUM CHLORIDE, U. TETRA METHYL AMMONIUM
CHLORIDE, U. TETRA ETHYL AMMONIUM CHLORIDE, U. CAESIUM CHLORIDE, U.
RUBIDIUM CHLORIDE, AND U. POTASSIUM CHLORIDE IN WATER.
(Rimbach, 1904.)
Formula^ of Double ^.o Gms. per 100 Gms. Sat. Sol.
Atomic Relation in Sol.
Solid Phase.
U02C12.2NH4C1.2H2O 15 40.67UO2+3.5iNH4+i9.i5Cl
IU02:z.59NH4:3.590 ^^Sgg
UO2Clj.2N(CH3)4O 29.8 19.85 " +io.44O2 =41.24*
iUO2: 4-020
Double salt
80.7 20.23 " +io.52O2 =41.91*
iU02: 3.980
*
UO2O2.2N(C2H5)4O 27.1 15-02
+ 7-8iO2 =37-i5t
iU02: 3-97C1
"
80.7 15.12
+ 7.78O2 =37-23t
iU02: 3-940
. (i
UO2O2.2CsO 29.75 22.11
UO2O2.2RbC1.2H2O 24.8 27.18
+22.5 Cs =56.04$
+16.6 Rb +i3.8O§
iUO2: 2.o7Cs
iU02:i.96Rb:3.9od
«
80.3 30.66
+ig.iRb +I5.8OH
iU02:i.98Rb: 3-95C1
u
U0202.2KC1.2H20 0.8 38.57
14-9 33-71
+13-590 + 3-86K
iUO2: 2.690 : o.69K
iUO2: 3.o6O :i.o6K
The double salt
I7-S 37-36
+i4.'soCl + 5-27K
iU02: 2.960 : o.96K
is decomposed
25 35.01
+15.260 + ... K
lUCy. 3-330 : I.33K •
by water at
4I-S 35-27
+15.920 + 7-39K
iU02: 3-440 : I.44K
temperatures
So 34-18
+16.560 + . . . K
iUO2:3.7id :i.7iK
below 60°.
60 34-19
+17.250 + 9.I4K
iU02: 3-850 : i.8sK
71.5 33.55
+I7.44C1 + Q.28K
iU02: 3-96C1 : I.96K
Double salt
78.5 35-26 +18.240 + 9-95K
iU02: 3-950 : I.95K
UO2C12.2N(CH3)4C1. f UO2C12.N(C2H6)4O. * UO2O2.2CsCl.
§ =57-9 gms. UO2O2.2RbO2. || =65.8 gms. UO2O2.2RbO2.
URANYL Sodium CHROMATE 2(UO2)CrO4.Na2CrC>4.ioH2O.
100 gms. sat. aqueous solution contain 52.52 gms. 2(UO2)CrO4Na2CrC>4 at 20°.
(Rimbach, 1904.)
URANYL IODATE UO2(IO3)2.
SOLUBILITY OF THE DIFFERENT CRYSTALLINE FORMS IN WATER AT 18°.
(Artmann, 1912-13.)
Gms. UO2(IO3)2
per loo Gms. H2O.
o . 1049
U02(I03)2.H20
«
UO2(IO3)2.2H2O
Appearance of Crystals.
Type I warty, later prismatic needles
Type II pyramids, sphenoids
0.1214
o . 2044
URANYL NITRATE UO2(NO3)2.6H2O.
SOLUBILITY IN WATER.
(Wasilieff, 1910.)
Gms. UO2(NO3)i
t°. per 100 Gms. Solid Phase.
Gms. UO2(NO3)2
t°. per 100 Gms.
Sat. Sol.
Sat. Sol.
- 1.6
IO . 83 Ice
— 2.2
48.77 .
— 2.1
12.24 "
0
49.46
~ 2.9
17.19 "
5-5
50-55
- 4.4
23.52
12.3
52.88
- 6
26 . 20
21. 1
55.98
- 7.9
32.53 "
25.6
57.17
— II .2
37.09 «
36.7
6l.27
-18.1
43.12 " +U01(N03)2.6H20
45-2
65.12
— 12. 1
45-53 U02(N03)2.6H20
51-8
67.76
Solid Phase.
UO2(NOS)2.6H20
loo gms. abs. acetone dissolve 1 .5 gms. UO2(NO3)2.6H2O at 12°. (de Coninck, 1900.)
100 gms. 85% alcohol dissolve 3.3 gms. UO2(NO3)2.6H2O at 12°.
Data for the densities of uranyl nitrate solutions in water and other solvents
are given byde Coninck (1900).
735
URANYL NITRATE
SOLUBILITY OF URANYL NITRATE IN ETHER.
(Lebeau, 1911.)
When a large excess of uranyl nitrate is shaken with ether at 7°, two liquid
layers are formed. The ethereal layer contains 59 gms. UO2(NO3)2 per 100 gms.
of solution and the aqueous layer contains 62.5 gms. per 100 gms. of solution. An
elevation of temperature was noted when ether and UO2(NO3)2.6H2O were mixed
at room temperature, therefore, indicating that solution is accompanied by com-
bination and elimination of the water of the salt.
URANYL DOUBLE NITRATES.
SOLUBILITY OF URANYL AMMONIUM NITRATE + URANYL NITRATE; U. CAESIUM
NITRATE + CAESIUM NITRATE; U. POTASSIUM NITRATE + POTASSIUM NITRATE
AND U. RUBIDIUM NITRATE + RUBIDIUM NITRATE IN WATER.
(Rimbach, 1904.)
Formulci of Stilt
Gms. per 100 Gms. Sat
. Solution.
Atomic Relation
'
'U02.
Total Salt.
in Solution.
UO2(N03)2.NH4NO3
0.5
29.71 + 2.92 NH4
= . .. i U
?2
i.47NH4:3.47NO3
«
24.9
36.46 + 3.54 "
= 68.95
1.46 " 13.46 "
(i
59
44.37 + 2.90 '
0.98 " : 2.98 "
U
80.7
44.95 + 2.98 '
= 78.95
i w : t
UO2(NO3)2.CsNO3
16
31. 39 + 6. 59 Cs
= 55-4
0.44 Cs
UO2(NO3)2.KNO3
o-5
2.37 NO3:o.37K
13
33.40 + 2.72 '
= . . .
2-57 ' ' :o.57'
25
37.07+4.01 '
= 64.82
i. 60 " =0.76'
45
42.18 + 5.16 '
= ...
2.84 " :o.84'
59
41.65 + 6.03 '
=
3 " :i '
80.6
43.71 + 6.38 '
= 80. i
3.01 ' n.oi1
U02.(N03)2.RbN03
25
35.41+4.65 Rbf
= 59.60
i. 40 " :o.45Rb
««
80
34.66 + 11.01 "
= 69.49
3 " n.oi "
* + 23-SN03. t + I9-74NO,.
URANYL OXALATE UO2.C2O4.3H2O.
100 gms. H2O dissolve 0.7401 gm. UO2C2O4.3H2O at 25°.
(Dittrich, 1899.)
EQUILIBRIUM IN THE SYSTEM URANYL OXALATE, AMMONIUM OXALATE
AND WATER.
(Colani, 1917.)
Results at 15°. Results at 50°.
Gms. per 100 Gms.
Sat. Solution.
Solid Phase.
Gms. per 100 Gms.
Sat. Solution.
Solid Phase.
0.47 o U02C204.3H20 i
7.19 2.14 " +(NH4)2(U02)2(Q!04)3.3H20 5-II
8.78 2.99 (NH4)2(U02)(C2O4)2.2H2O + " 19.89
Q.66 6.43 " +(NH4)2C204.H20 23.82
O 3-^9 (NH4)2C2O4.H2O O
Two determinations at 75° are also given.
EQUILIBRIUM IN THE SYSTEM URANYL OXALATE, POTASSIUM OXALATE
AND WATER.
(Colani,
O U02.C204.3H20
1-36 " +(NH4)2(U02)2(C204),
8.52 (NH4)2(U02)(C204)2+ "
15.90 " +(NH4)2C204.H20
9-36
Results at 15°.
Results at 50°.
Gms. per 100 Gms.
Sat. Solution.
Solid Phase.
U02C204.3H20
" +K2(U02)2(C204)3.4H20
" +Ke(U02)2(C204)B.ioH20
K2C2O4.H2O+
K2C20«.H20
Gms. per 100 Gms.
Sat. Solution.
Solid Phase.
" +K,(U02)2(C204)8.4H20
K2(U02)(C204)2+ "
" +K,(U02)2(C204)6.ioH2O
K2C204.H20+
U02C204.
0.47
1-34
3.89
3.76
0.10
0
K2c2o4:
0
0.42
1.83
1.85
24.30
24.09
U02P204.
I
3-45
9.82
9-59
I. 22
0
K2Q04.
0
I. II
4.83
5-6l
32.65
32.75
URANYL OXALATE
736
SOLUBILITY OF URANYL OXALATE IN AQUEOUS SODIUM OXALATE AT 25°.
(Dittrich, 1899.)
Cms. UO2.C2O4.3H2O
per 100 cc. Sat.
Solution.
2.0125
0.9867
0.6059
Gms. Na2C2O4
per lop cc.
Solution.
0.6706
0-3353
0.2235
URANYL Ammonium PROPIONATE
URANYL Potassium PROPIONATE UO2(C3H5O2)2.KC3H6O2.
100 gms. aq. solution contain 16.48 gms. 2UO2(C3H5O2)2.NH4C3H6O2 at 29.8°.
100 gms. aq. solution contain 2.362 gms. UO^CsHsO^ + 0.82 grn. KCsH5O2
at 29.4°, atomic relation, i: 1.29. (Rimbach, 1904.)
URANYL SULFATE UO2SO4.3H2O.
SOLUBILITY IN SEVERAL SOLVENTS.
(de Coninck, 1901, 1903.)
Gms. UO2SO4.-
t°. sH2O per zoo
Gms. Solvent.
13.2 18.9
15-5 20.5
12.3
2.6
30
Solvent
Water
Water
16.2% Alcohol 10
85% Alcohol 1 6
Cone. HC1 13
Solvent.
Cone. HBr (J=i.2i)
Cone. HN03
Cone. H2SO4 (d= 1.138)
i Vol. HCl+i Vol. HNO3
Selenic Acid (d= 1.4)
Gms. UO2S04.-
t°. 3H2O per 100
Gms. Solvent.
16.8
12
12
13
16
IS
9.1
24-3
18
27
URANYL Potassium SULFATE U02SO4.K2SO4.2H2O.
100 gms. sat. aq. solution contain 10.41 gms. UO2SO4.K2SO4 at 25° and 23.13
gms. at 70.5°. (Rimbach, 1904.)
SOLUBILITY OF UO2SO4.2K2SO4.2H2O + UO2SO4.K2SO.2H2O IN WATER.
Gms. per 100 Gms. Solution. Atomic Relation in Sol. Mol. % in Solid Phase.
UO,
14 0.85
50 6 . 70
80 14. 29
K.
4.19
8.15
8-54
S04.
5-71
12.37
15-53
U02
. K.
S04.
I
35-75
18.88
I
5.20
8.40
I
4-i3
3.06
Mono Salt. Di Salt.
29 71
76 24
12 88
URANIUM SULFATE (ous) U(S04)2.
i SOLUBILITY IN WATER.
(Giolitti and Bucci, 1905.)
Gms. U(SO4)2
Solid Phase. t°. per 100 Gms.
Sat. Sol.
93 63 . 2
24 9.8
37 8.3
48.2 8.1(7.8)
63 7.3
18
25.6
37
48.2
62
Gms. U(SO4)2
per loo Gms.
Sat. Sol.
10. 17
I3-32
19.98
28.72
36.8
Solid Phase.
U(SO4)2.8H2O
The determinations were made with difficulty on account of the considerable tend-
ency towards formation of basic sulfate and simultaneous clouding of the solution.
APPROXIMATE SOLUBILITY OF URANIUM SULFATE, IN AQUEOUS SOLUTIONS.
(de Coninck, 1903.)
Solvent.
Water n
Dilute HC1 (1:4) 9
Dilute HN03 (1:4) 10.5
Gms.
U(S04)2.4H2O
per 100 Gms.
Solvent.
23.2
17.2
18.2
Solvent.
Gms.
U(S04)2.4H20
per 100 Gms.
Solvent.
Dilute Selenic Acid (1:4) 11.4 21.7
Dilute H2SO4 (1:4) 10 15.6
Dilute Alcohol (i: 4) 11.3 12.3
737
UREA
UREA CO(NH2)2.
SOLUBILITY IN WATER AND IN ALCOHOLS.
(Campetti, 1902; Speyers, 1902.)
NOTE. — Speyer's original results are in terms of Mols. CO(NH2)2 per 100 mols.
H2O at irregular temperatures.
In Water. In Methyl Alcohol. In Ethyl Alcohol.
t°.
Wt. of i cc.
Solution.
Cms. CO(NH2)2 per Wt. of i cc.
100 Cms. H2O. Solution.
Gms.
CO(NH2)2
per 100 Gms.
Gms.
Wt. of ice. CO(NH2)a
Solution, per 100 Gms
CH3OH.
(J2H5OH.
o
I .121
55-9
0.861
13.8
0.8213
2-5
IO
I-I34
66.0
8S!o(C)
0.863
16.0
0.8l4
3-5
20
1.146
79.0
io8.2(C)
0.869
20.0
0.809
5-o
3°
I .156
93-o
0.876
24.0
0.8o6
6-5
40
I .165
106.0
. . .
0.890
30.0
0-804
8-5
5°
I-I73
I2O-O
0.908
37-o
0.803
10.5
60
I.lSo
132.0
0.928
47.0
13.0
70
I.lSy
145.0
17-5
100 gins. abs. methyl alcohol dissolve 21.8 gms. CO(NH2)2 at 19.5°.
loogms.abs. ethyl alcohol dissolve 5.06 gms. CO(NH2)2at 19.5°. (de Bmyn, 1903.)
SOLUBILITY OF UREA IN ALCOHOLS.
(Timofeiew, 1894.)
Gms.
100 Gms.
olvent.
Isopropyl Alcohol
Alcohol.
t°.
per zoo Gn
Solvent.
Methyl Alcohol
— 12
II
tt
O
14.2
"
19
20.9
M
40
36.4
"
62
66.6
"
71
107.4
Ethyl Alcohol
- 9
2.69
u
o
3-26
"
18
5
"
41
9-45
"
60
16.3
tt
81
30.8
Propyl Alcohol
0
1.65
tt
20
2.56
tt
40
5-12
"
60
7.72
tt
80
12.28
"
98
18.06
Alcohol.
Isobutyl Alcohol
Isoamyl Alcohol
tt
it
(C
It
Capryl Alcohol
a
Ally Alcohol
SOLUBILITY OF UREA IN ETHYL ACETATE CONTAINING SMALL AMOUNTS
Gms. CCXNHj)
t°.
per 100 Gms.
Solvent.
19
4 5.76
20
6.17
Si
23.46
0
1. 01
19
1.65
41
3-12
60
4.40
80
6-34
98
10
20
1.18
60
3-41
80
4.88
83
5-24
6.15
10
4 0.56
OS
2
19
4 9-37
OF WATER
AT 25°.
(Lewis and Burrows, 1912.)
Gms. H2O per 100
Gms. Urea
Gms. H2O per
Gms. Urea
Gms. Solvent.
(Ethyl Acetate +H2O).
per TOO Gms.
Sat. Sol.
100 Gms. Solvent.
(Ethyl Acetate +HjO).
per too Gms.
Sat. Sol.
0
O.oSo
1.677
0.308
0.652
0.148
2.0O6
0.328*
I. 112
0.198
2.138
0.342
1.638
0.296
3-234
o-343t
A second liquid phase was suspected here.
t A second liquid phase could be distinguished.
UREA
738
SOLUBILITY OF UREA IN ETHYL ETHER.
(Gortner, 1914.)
When 0.3255 gm. urea was extracted in a Soxhlet apparatus with anhydrous
ether for 48 hours, the extract was found to contain 0.072 gm. urea. An approxi-
mate estimate, based on the volume of liquid and the number of siphonings per
hour indicates a solubility of 0.0004 gm. urea per 100 cc. of ether.
100 gms. glycerol dissolve about 50 gms. urea at 15°.
100 gms. pyridine dissolve 0.96 gm. urea at 20-25°. (Dehn, 1917.)
100 gms. aq. 50% pyridine dissolve 21.53 gms. urea at 20-25°.
Diphenyl UREA.
100 gms. H2O dissolve 0.015 g"1' diphenyl urea (sym or uns.?) at 20-25°.
" pyridine dissolve 6.85 gms. diphenyl urea (sym or uns.?) at 20-25°.
" aq. 50% pyridine dissolve 5.3 gms. diphenyl urea (sym or uns.?) at
20-25°. (Dehn, 1917.)
ThioUREA NH2.CS.NH2.
loo gms. H2O dissolve 9.1 gms. thiourea at 20-25°.
" pyridine dissolve 12.5 gms. thiourea at 20-25°.
" aq. 50% pyridine dissolve 41.2 gms. thiourea at 20-25'
(Dehn, 1917.)
Allyl ThioUREA (Thiosinamine) NH2.CS.NH.C3H6.
100 cc. H2O dissolve about 5.9 gms. NH2.CS.NH.C3H6 at 15-20°.
100 cc. 90% alcohol dissolve about 50 gms. NH2.CS.NH.C3H6 at 15-20°.
(Squire and Caines, 1905.)
Phenyl ThioUREA (Phenyl thiocarbamide) CS.NH2.NHC6H6.
SOLUBILITY IN WATER.
(Rothmund, 1900; Biltz, 1903; Hollman and Antusch, 1894; Bogdan, 1902-03.)
One liter aq. solution contains 2.12 gms. CS(NH2).NHC6H6 at 20° (B.), (R.)
and 2.4 gms. at 25°. (H. and A.). Bogdan gives 2.547 gms. at 25°.
SOLUBILITY OF PHENYL THIOUREA AT 25° IN AQUEOUS SOLUTIONS OF.
Potassium Nitrate.
Sodium Nitrate.
(Bogdan, 1902-03.)
(Bogdan, 1902-03.)
Gms. Mols.
KNOa per
jooo Gms.
HzO.
Gms. per
1000 Gms^. H2O.
Gms. Mols.
NaNO3 per
jooo Gms.
H20.
Gms. per
looo Gms. H2O.
KNO,.
CS(NH2)
.NHCftHg.
NaNO3.
CS(NH2)
NHQ»H5.
1.045
0.5123
O.2O26
0.1007
105-7
5I-84
20.50
IO.I9
2-38
2.48
2-54
2-56
1.024
0.5065
0.2031
0-0986
87.14
43.10
17.28
8-39
2.26
2 .46
2.51
2-53
0.0503
0-0333
5-09
3-36
2-55
2-55
0-0540
0-0335
4-59
2.84
2-54
2-54
739
Phenyl ThioUREA
SOLUBILITY OF PHENYL THIOUREA IN AQUEOUS SALT SOLUTIONS AT 20°.
(Biltz, 1903; Rothmund, 1900.)
Millimols and the Equivalent Cms. CSCNH^NHCjHs Dissolved per Liter of
Aqueous Salt Solution of Concentration:
0.125 Normal
0.25 Normal
0.5 Normal.
i Normal
Millimols.
Gms.
Millimols.
Gms.
Millimols.
Gms.
Millimols.
Gms.
IAIO,
12
•95
1.97
12.82
I .96
12.03
I
•83
10
.69
1.61
NH4N03
14
2.15
14.4
2.21
14-53
2
.22
14
.91
2.27
i(NH4)2S04
J3
•51
2 -05
12.84
1.96
11.78
I
•79
9
.98
1.52
iBaC!2
13
.12
1-99
12 .92
i-97
12.22
I
.86
10
.44
1 -59
iBa(N03)2
13
.98
2.13
13.98
2.13
13.90
2
.12
CsNO3
14
•53
2 .21
14.90
2.27
15.23
2
•33
.
..
LiNO3
13
.96
2.13
13.96
2.13
13-93
2
.12
13
•73
2.10
£MgSO4
*3
.40
2.04
12.78
I .95
n-54
I
•75
9
•43
i-43
KC2H3O2
.40
2 .04
12-95
1-97
12.14
I
•85
10
•74
1.62
KBr
13
•5°
2 .05
13-35
2 .04
12.80
X
•95
ii
.76
1.79
KC103
I3
.86
2. II
13.60
2 .06
13.12
I
•99
KC1
*3
.40
2 .04
12.73
1.94
12.19
X
•85
10
•54
i. 60
Kl
14
.12
2.15
14.48
2 .21
I4-31
2
.18
14
.60
2.23
KNO3
13
.89
2.12
I3-85
2 .11
I3-52
2
•05
12
.82
i .96
KN02
14
•52
2.21
14.65
2.23
13.80
2
.11
12
.51
1.92
JK2SO4
13
•25
2 -03
12.49
I.9I
ii .11
I
.69
8
•73
i-33
RbN03
14
.22
2.l6
14.44
2.19
14-39
2
.18
14
.22
2.17
iNa2C03
13
.29
2 .04
12.52
I.9I
ii .05
I
.68
8
•58
1.32
NaClO3
13
•75
2 .09
I3-65
2.08
13.07
I
.98
12
.21
1.86
NaClO4
14
2.15
14.05
2.14
I3-58
2
.06
12
•56
1.92
NaCl
.28
2 .02
12.83
i-95
ii .90
X
.81
10
.02
1.52
Nal
13
.98
2.13
14.07
2.14
14.29
2
.18
13
.96
2.13
NaNO3
•94
2.12
13-77
2.10
13 .32
2
.04
12
•57
1.92
NaNO2
14
•34
2.18
13.82
2 .11
13.06
I
.98
II
•52
i .75
JNa2S04
13
2 .00
12.35
1.87
10.85
I
•63
8
•30
1.27
SOLUBILITY OF PHENYL THIOUREA IN ETHYL ALCOHOL SOLUTIONS OF
SEVERAL SALTS AT 28°.
(Thorin, 1915.)
Normality
Mols.
Normality
Mols.
Salt.
of Salt
in
NHj.CS.NHQHg
per 100 Gms.
Salt.
of Salt
in
NHs.CS.NH.QHj
per too Gms.
QHBOH.
Sat. Sol.
QHBOH.
Sat. Sol.
None
(pure C2H5OH)
o . 2065
Nal
0.043
O.2I02
LiCl
0.168
0.2274
n
0.086
0.2148
tt
o-337
0.2360
t(
0.172
0.2198
(C
0.673
o . 2440
n
0-343
0.2271
tc
1.346
0.2494
it
0.685
0.2359
CaCl-
0.061
0.2IOI
NaBr
0.022
o . 2098
ft
0.122
0.2135
tt
0.043
0.2194
tt
0.244
0.2194
tt
0.086
0.2165
tt
0.487
0.2279
tt
O.I72
0.2257
u
0.975
0.2372
»
Phenyl ThioUREA
740
SOLUBILITY OF PHENYL THIOUREA IN MIXTURES OF ETHYL ALCOHOL
AND WATER AT 25°.
(Holleman and Antusch, 1894.)
Cms.
Vol. CS(NH2) Sp. Gr.
per cent NHCsHs of
Alcohol, per 100 Cms. Solutions.
Solvent.
Cms.
Vol. CS(NH2) Sp.Gr.
per cent NHC«H5 of
Alcohol, per 100 Cms. Solutions.
Solvent.
100
3-59
95
4-44
0.8200
90
4.69
0.8389
85
4-99
0.8544
80
4-70
0.8679
75
4-45
0.8810
70
3-92
0.8915
65
3-40
0.9018
60
2.80
0.9128
50
1.87
0.9317
40
i -13
o . 9486
25
0.56
0.9679
IS
0.38
0.9788
o
0.24
0.9979
See remarks under a. acetnaphthalide, p. 13.
SOLUBILITY OF PHENYL THIOUREA IN AQUEOUS SOLUTIONS OF PROPYL
AND OF ETHYL ALCOHOL AT 25°.
(Bogdan, 1902-03.)
In Aq. Propyl Alcohol. In Aq. Ethyl Alcohol.
G. Mols.
Gms. per loop Gms.H2O
G. Mols.
Gms. per 1000 Gms. H2O
CjHrOH per
1000 GDIS.
H2O.
C3H7OH.
CS(NH2)'
NHC6H6.
C2HfiOH per
1000 Gms.
H20.
C2H5OH.
CS(NH2)
1-035
62 .IO
3.587
I .IOIO
49.60
3-*93
0.5448
32.688
3.124
0-5355
24.12
2.931
0.1059
6-354
2.643
o . 1094
4-932
2 .629
0.05526
3-3l6
2-599
0.05018
2 .26
2.589
0-04854
2 .912
2.586
0.03271
1-473
2-577
In Propyl Alcohol
at o°.
i .000
60.06
I .21
o.ioo
6.01
1.047
SOLUBILITY OF PHENYL THIOUREA IN AQUEOUS SOLUTIONS OF ACETONE,
MANNITOL, CANE SUGAR, DEXTROSE, AND UREA.
(Bogdan, 1902-03.)
Aqueous
Non Electro-
Gms. per 1000
to H?0
Gms.
Aqueous
Non Electro-
to
Gms. per 1000 Gms.
H20.
lyte.
Non Elec-
trolyte.
SSH<NC§fl
lyte.
•
Non Elec-
trolyte.
CS(NH2)
NHC6H6.
(CH3)2CO
25
7
.478
2
.667
C6H1206
25
180
.40
3
.042
tt
tt
2
.513
2
•579
a
tt
90
.46
2
•83
a
u
I
.908
2
•573
11
11
29
.29
2
.69
C.H8(OH),
It
182
.11
3
.04
"
11
18
.01
2
•654
tt
(I
91
•05
2
.78
"
"
9
•554
a
.603
C^H^On
25
338
.6
3
•457
CO(NH2)2
ft
63
.08
3
.306
it
M
170.4
3
.015
tt
11
29
•93
2
.892
tt
tt
34-36
2
•634
(I
It
6.132
2
.6l8
tt
tt
18
.28
2
•596
tt
tl
4
.942
2
-605
»t
tt
10
.09
' 2
•572
ft
It
2
.009
2
•572
*
0
342
.18
I
.420
tt
0
60
.11
1
.310
U
tt
34
.22
I
.044
tt
tt
6
.01
I
.048
741
UREIDE
UREIDE OF GLUCOSE CH2OH.(CHOH)4.CH : N.CO.NH2.
100 gms. absolute ethyl alcohol dissolve 0.04 gm. ureide of glucose at 25°.
85,6% . " " 0.73 "
methyl alcohol
0.22
(Schoorl, 1903.-)
URETHAN (Ethyl Carbamate) NH2.CO2.C2H6. (See also p. 296.)
SOLUBILITY OF URETHAN IN SEVERAL SOLVENTS.
(Speyers, 1902.)
Interpolated and calculated from the original results which are given in terms
of molecules urethan per 100 mols. solvent.
Solubility in Water.
Solubility in Methyl Alcohol.
/ —
Mols.
Gms
r~~
\i7*. e
Mols.
Gms.
t°.
Wt. of
I CC.
Solu-
.• _
CO(NH2)
OC2H6 per
100 Mols.
CO(NH2)
OC2H6per
100 Gms.
Wt. or
I CC.
Solu-
CO(NH2)
OC2H5per
100 Mols.
8§»
zoo Gms.
tion.
H20.
H20.
tion.
CH3OH.
CH3OH.
o
1.023
3-6i
I7.8
0.956
31.18
86.76
IO
1-033
6.0
29.7
0-977
41 -o
II4-I
15
i .042
15.0
74-2
0.989
47-5
I32.I
20
i .060 •
31.0
153-3
I -OOO
54-5
i$* -7
25
1.073
50.0
247-3
I.OI3
62.5
173-9
3°
1.078
65.0
321.4
I .024
72.0
200.3
40
i .065
77.0
380.7
1.045
89.0
247-7
Solubility in Ethyl
Alcohol.
Solubility
in Propyl
Alcohol.
t°.
Wt. of
I CC.
Solu-
A" _
Mols.
CO(NH2)
OC2H5per
100 Mols.
Gms.
CO(NH2)
OC2H5 per
loo Gms.
Wt.of
I CC.
Solu-
4.* _
Mols.
CO(NH2)
OC2HS per
100 Mols.
Gms.
CO(NH2)
OC2H5 per
100 Gms.
lion.
C2H5OH.
C2H5OH.
tion.
CaHyOHo
C-jHyOH.
o
0.8914
23.91
46.26
0.880
19.48
28.9
IO
0.930
36.0
69.6
0.906
31.0
46.0
15
0.950
43-o
89.2
0.923
4O.O
59-3
20
0.968
50.0
96.7
0.942
51.0
75-7
25
0.985
59-o
II4.I
0.963
6o-O
89.0
30
i .001
70.0
135-4
0.983
68.0
100.9
40
I-°35
88.0
170.2
1.025
85.0
126.1
Solubility in Chloroform.
Solubility in Toluene.
t°
Wt. of
I CC.
Solu-
Mols.
CO(NH2)
OC2H6per
100 Alois.
Gms.
CO(NH2)
OCsHsper
100 Gms.
Wt.of
I CC.
Solu-
Mols.
CO(NH2)
OC2H6 per
100 Mols.
Gms.
CO(NH2)
OCsH per
loo Gms.
tion.
CHC13.
CHCU.
tion.
CeHsCHa.
CcHsCHg.
0
.404
27.56
20. 6
0.887
1-77
I.7I
10
•340
41
30.6
0.874
5-o
4.84
X5
.310
46
34-4
0.875
10. 0
9.68
20
.280
53
39 6
0-883
16.0
15.48
25
.240
60
44-8
0.902
25.0
24.18
30
.203
67
50.0
0.927
44.0
42.58
40
I.I25
80
59-7
o-995
85.0
82.24
100 gms. sat. solution in liquid CO2 contain 4 gms. urethan at the critical tem-
perature, 23.5°; at 30.5° the mixture separates with two layers. (Buchner, 1905-06.)
100 gms. pyridine dissolve 21.32 gms. urethan at 20-25°.
i oo gms. aq. 50% pyridine dissolve 101.1 gms. urethan at 20-25*
(Dehn, 1917.)
URETHAN 742
SOLUBILITY OF URETHAN DERIVATIVES IN WATER.
(Odaira, 1915.)
Gms. Cmpd.
Name. Formula. t°. per 100 Gms.
H20.
Detonal (Diethyl Aceturethan) (CjHs^CH.CO.NH.CO.OCjHs ... 0.526
Epronal (Ethylpropyl Aceturethan) (QH6)(C3H7)CH.CO.NH.CO.OC2H5 cold 0.143
Dipronal (Dipropyl Aceturethan) (C3H7)CH.CO.NH.CO.OC2H6 20 0.040
Probnal (Propylbutyl Aceturethan) (C3H7)(C4H9)CH.CO.NH.CO.OC2H5 20 0.032
Dibnal (Dibutyl Aceturethan) (C4H9)2CH.CO.NH.CO.OC2HB ... 0.008
Oenanthyl Urethan CH3(CH2)6CO.NH.CO.OC2H5 ... 0.021
n Isoamyl Urethan (C2H5)2CH.NH.CO.OC2H6 20 0.410
a Bromethyl Propyl Aceturea (CiHsXCsH^CBr.CO.NH.CO.NHj 20 0.041
DISTRIBUTION OF URETHAN DERIVATIVES BETWEEN WATER AND OLIVE OIL.
Gms. Cmpd. per Dist. Ratio
Name. Formula. t°. - '°°^ - :> Conc-°ii
H2O Olive Oil 7^— --
Layer. Layer. Conc-H2o
Ethyl Urethan NHiCOOQH, ord. 4.52 0.615 0.136(1)
Methyl Urethan NH2COOCH3 ord. 7.50 0.275 0.037(1)
Aceturethan CHsCONH.COOCjHs 17-20 2.94 0.389 0.132(2)
Epronal (QHsXCjHOCH.CO.NH.CO.OCjHj ". 0.076 0.257 3.3(2)
Detonat (QHj.CH.co.NH.co.OCiH. "
Veronal (diethylbar- [ rrvxrwrm r <r H ^ " o. 180 o. 020 o. n (2)
bituricacid) } COCNHCOWXCqW, \o.M 0.032 0.12(2)
(i) Baum, 1899; H. von Meyer, 1909. (2) Odaira, 1915.
URIC ACID
SOLUBILITY IN WATER.
(Blarez and Deniges, 1887; at 15° Magnier, 1875.)
Gms. CsJL^Oa. Gms. C6H^tOa Gms.
t*. per 100 Gins. t°. per 100 Gms. t°. per 100 Gms.
H20. H30. H20.
O 0.002 30 0.0088 70 0-0305
10 0.0037 4° 0-0122 80 0-0390
15 O.OO53 50 O.OI7O 9O 0-0408
20 0.006 60 0-0230 loo 0-0625
One liter of very carefully purified CO2 free water dissolves 0.0253 gm. uric
acid at 18°. Constant agitation and temperature were employed. With finely
divided uric acid, saturation was reached after one hour. The amount dissolved
was determined by the difference in weight between the amount of sample taken
and that remaining undissolved. (His, Jr. and Paul, 1900.)
One liter of pure CO2 free water dissolves 0.0649 Sm- uric acid at 37°. The
amount dissolved was determined by difference and only 20-25 minutes agitation
allowed for saturation. It is stated that on long contact with water, the uric
acid breaks down and the solubility and conductivity increase directly with time.
(Gudzeit, 1909.)
One liter of water dissolves 0.0645 grn- uric acid at 37°. (Bechhold and Ziegler, 1910.)
One liter of serum dissolves 0.9 gm. uric acid at 37°.
743 URIC ACID
SOLUBILITY OF URIC ACID IN AQUEOUS SOLUTIONS OF ACID AT 18°.
(His, Jr. and Paul, 1900.)
Concentration of Aq. Acid. Gms. Uric Acid
Acid. t- • per 1000 cc.
Normality. Per cent. Sat Sol.
Hydrochloric i 3.65 0.0236
3-75 13-69 0.0263
6.24 22.77 0-0375
Sulfuric i 4.9 0.0227
3.2 15.67 0.0205
6.4 31-34 0.0183
Additional data for the solubility of uric acid in aqueous sulfuric acid are given
by Tafel (1901). A saturated solution of crystallized uric acid in 80 wt. per cent
aqueous H2SO4 was prepared by warming to about 120° and allowing to stand.
Portions of the clear solution were diluted with increasing amounts of water and
the mixtures allowed to stand many days in closed flasks which were frequently
shaken. The precipitated uric acid was then filtered off and weighed and the
amount remaining in solution calculated by difference. The following results
were obtained.
Wt. % of aq. H2SO4 72.5 70.5 68 66.5 62.5 59.5
Gms. uric acid per 100 gms.
aq. H2S04 6.45 3.85 1.60 0.64 0.35 0.312
An approximate determination of the solubility of uric acid in alcohol by ex-
traction in a Soxhlet apparatus, gave 0.00008 gms. per 100 cc. A similar determi-
nation with ether as solvent, gave negative results. (Gortner, 1914.)
IOO gms. 95% formic acid dissolve 0.04 gm. uric acid at 20°. (Aschan, 1913.)
pyridine dissolve 0.21 gm. uric acid at 20-25°. (Dehn, 1917.)
" aq. 50% pyridine dissolve 0.75 gms. uric acid at 20-25°. "
VALERIC ACID n CH3(CH2)3COOH (n Propyl Acetic Acid).
When valeric acid is shaken with water at 16°, two layers are formed.
100 gms. of the aqueous layer contain 3.4 gms. CHsCCt^sCOOH.
100 gms. of the acid layer contain 90.4 gms. CHsCCf^sCOOH.
/Lieben and Rossi, 1871.)
DISTRIBUTION OF VALERIC ACID BETWEEN BENZENE AND 95.8% SULFURIC
ACID.
(Gurwitsch, 1914.)
The mixtures were made at o° and brought to equilibrium by shaking for 5
minutes at 18°, and allowing to stand over night.
", Gms. Valeric Acid per too Gms. Gms. Valeric Acid per 100 Gms.
Benzene Layer. H2SO4 Layer. • Benzene Layer. H2SO4 Layer.
7.60 46.4 I 36.7
4.78 44.8 0.58 35.2
3.64 43.5 0.29 32.7
2.61 41.4 0.20 30.7
1.62 39.5 0.04 26.1
1.48 38.1 0.007 23-8
The coefficient of distribution of isovaleric acid between benzene and water at
room temperature is, cone, in CeH6 -r cone, in HjO = 2.744. (King and Narracott, 1909.)
VALERAMIDES
744
DISTRIBUTION OF VALERAMIDES BETWEEN WATER AND OLIVE OIL AT 15°.
(Harrass, 1903.)
Amide.
Formula.
Valeramide
Valerethylamide
Valerdiethylamide
Valerdimethylamide
Lactdiethylamide
CH3(CH2)3CONH2
CH3(CH2)3CONH(C2H5)
CH3(CH2)3CON(C2H5)2
CH3(CH2)3CON(CH3)2
CH3CHOHCON(C2H5)2
Gms. Cmpd. per
per 100 cc.
Ratio
Conc.oU
Water
Layer.
Olive Oil
Layer.
Conc.H2o
0.769
O.24I
0-3I3
I .029
O.26l
0.254
0.231
1-339
5-797
O.QII
o-379
0.416
1.256
0.194
0.154
VANILLIN CeHs.CHO.OCHg.OH, 1.3.4.
100 gms. H2O dissolve I gm. vanillin at 20-25°.
100 gms. pyridine dissolve 316 gms. vanillin at 20-25°.
(Dehn, 191?-)
DISTRIBUTION OF VANILLIN BETWEEN WATER AND ETHER AT 25°.
(Marden, 1914.)
Dist. Coef.
0.108
O.IIO
Gms. Vanillin per 100 cc.
H2O Layer. Ether Layer.
0.0l64 0.1294
O.O242 0.1854
0.0403 0.3310 O.IO4
Fusion-point data for mixtures of vanillin and orthovanillin are given by
Noelting (1910). Qualitative solubilities of orthovanillin in a number of solvents
are also reported. Data for the sintering, melting and clear liquid points for
mixtures of vanillin and an extensive series of compounds are given by Lehmann
(1914).
VERATRINE
SOLUBILITY IN SEVERAL SOLVENTS.
Solvent.
Water
Water
3% H3B03 in Aq.
50% Glycerol
Aniline
Pyridine
Piperidine
Diethylamine
Oil of Sesame
t°.
Gms. Veratrine
per loo Gms.
Solvent.
25
0.057
20
O.II4
ord.
6
20
37
20
20
'75
83
20
271
20
i-39
Authority.
(U. S. P. VIII.)
(Zalai, 1910.)
(Baroni & Barlinetto, 1911.)
(Scholtz, 1912.)
(Zalai, 1910.)
VERATROLE Ce
F.-pt. data for mixtures of veratrole and p xylene are given by Paterno and
Ampola (1897).
VERONAL (Diethylbarbituric Acid) CO< (NHCO)2> C(C2H6)2. See also p. 742.
100 cc. H2O dissolve 0.625 gm. veronal at 15-20°. (Squire & Caines, 1905.)
100 cc. 90% alcohol dissolve 11.7 gms. veronal at 15-20°.
100 cc. ether dissolve 8.7 gms. veronal at 15-20°. "
VESUVIN.
loo gms. water
pyridine
. 50% pyridine
dissolve 8.5 gms. vesuvin at 20-25°. (Dehn, 1917.)
i. K.t»«
31-4
745 WATER
WATER H2O.
SOLUBILITY OF WATER IN BENZENE, PETROLEUM AND PARAFFINE OIL.
(Groschuff, 1 91 1.)
The synthetic, sealed tube method was used and the experiments were made
with very great care. The mixtures were first superheated sufficiently to bring
all the water into solution and then cooled until a fine mist was formed. The
temperature of appearance and disappearance of this fine mist was determined re-
peatedly. The benzene was of dm = 0.8799. The petroleum was American
water white, of d = 0.792. It was freed from HzO by distilling 3 times from
melted Na and boiled at 190-250° at atmospheric pressure. The paraffine oil
was first heated to 120-130° and then distilled twice under vacuum over melted
Na and once without Na. Its du = 0.883 and b.-pt. was 2OO°-3OO° at 10 mm.
pressure.
Results for:
H2O + Benzene.
H20 + Petroleum.
H2O + Paraffine Oil.
t°.
+ 3
23
40
55
66
77
Cms. H2O
per 100 Gms. Sol.
0.030
0.061
0.114
0.184
o-255
o-337
t°.
+ 18
23
30
36
53
Gms. H2O
per 100 Gms. Sol.
0.0012
0.005
O.OO7
0.008
O.OI2
O.O26
t°.
59
61
66
79
85
94
Gms. H2O
per 100 Gms. Sol.
0.031
0.035
0.043
0.063
0.075
O.OQ7
''•per
+ 16
5°
65
73
77
94
Gms. H2O
100 Gms. Sol.
0.003
O.OI3
0.022
O.O3O
0.035
0.055
Observations on the solubility of water in essential oils are given by Umney and
Bunker (1912).
XENON Xe. SOLUBILITY IN WATER.
(von Antropoff, 1909-10.)
The results are in terms of the coef. of absorption /3, as defined by Bunsen (see
p. 227) and modified by Kuenen in respect to the substitution of mass for volume
of water.
t°. 0°. 10°. 20°. 30°. 4°°. 50°.
Abs.Coef.j9 0.2180 0.1500 0.1109 0.0900 0.0812 0.0878
NitroXYLENES.
loo gms. 95% formic acid dissolve 0.71 gm. trinitro-w-xylene (m. pt. 173°) at
18.5°. (Aschan, 1913.)
F.-pt. data for mixtures of 2.3, dinitro-£-xylene and 2.6, dinitro-£-xylene are
given by Blanksma (1913).
XYLENOL 1.3.4, C6H3.(CH3)2.0H.
MISCIBILITY OF AQUEOUS ALKALINE SOLUTIONS OF XYLENOL WITH SEVERAL
ORGANIC COMPOUNDS, INSOLUBLE IN WATER.
(Sheuble, 1907.)
To 5 cc. portions of aq. KOH solution (250 gms. per liter) were added the given
amounts of the aq. insoluble compound from a buret and the xylenol, dropwise,
until solution occurred. Temperature not stated.
Composition of Homogeneous Solution.
cc. Aq. KOH. cc. Aq. Insol. Cmpd. Gms. Xylenol.
5 2 (= 1.64 gms.) Octyl Alcohol (i) i
S 5 ( = 4-io « ) 1.7
5 2 (=1.74 " ) Toluene 4.1
5 3 (=2.61 " ) 5
(i) The normal secondary octyl alcohol, i.e., the so-called capryl alcohol, CH3(CH2)5.CH(OH)CH,.
YTTERBIUM 746
YTTERBIUM CobaltiCYANIDE Yb2(CoC6N6)2.9H2O.
1000 gms. aqueous 10% HC1 (^15 = 1.05) dissolve 0.38 gm. of the salt at 25°.
(James and Willand, 1916.)
YTTERBIUM OXALATE Yb2(C2O4),.ioH2O.
SOLUBILITY IN WATER AND IN SEVERAL AQUEOUS SOLUTIONS.
Aqueous- Solution of: Per cent Cone. +<> Gms. YbztQOOs A fl, •«.
ofAq.Sol. * per 100 cc. Solvent. Authonty.
Water ... 25 O.OOO334 (Rimbach and Schubert, 1909.)
(NH4)2C2O4.H2O 3.26 Ord. 0.095 (Cleve, 1902.)
Methylamine Oxalate 20 5 . 24* (Grant and James, 1917.)
Ethylamine Oxalate 20 5.86*
Triethylamine Oxalate 20 2.05*
Sulfuric Acid (i n) 4.9 °-372 (Cleve, 1902.)
* The authors do not state whether their figures are for anhydrous or hydrated salt.
YTTERBIUM Dimethyl PHOSPHATE Yb2[(CH3)2PO4]6.
loo gms. H2O dissolve 1.2 gms. Yb2[(CH3)2PO4]6 at 25° and 0.25 gm. at 95°.
(Morgan and James, 1914-)
YTTERBIUM SULFATE Yb2(S04)3.8H2O.
SOLUBILITY IN WATER.
(Cleve, 1902.)
Gms. Yb2(S04)3
t°. per 100 Gms.
H20.
80 6.92
90 S-83
100 4-67
YTTERBIUM Bromonitrobenzene SULFONATE Yb(C6H3Br.NO2.SO3f 1.4.3)3.-
I2H2O.
100 gms. sat. solution in water contain 7.294 gms. of the anhydrous salt at 25°.
(Katz and James, 1913.)
YTTRIUM CHLORIDE YC13.
100 gms. alcohol dissolve 61.1 gms. YC13 at 15°. (Matignon, 1906.)
60.5 gms. YC13 at 2O°. (Matignon, 1909.)
pyridine dissolve 6.5 gms. YC13 at 15°. (Matignon, 1906.)
YTTRIUM CobaltiCYANIDE Y2(CoC6N6)2.9H2O.
1000 gms. aq. 10% HC1 (d^ — 1.05) dissolve 2.78 gms. of the salt at 25°.
(James and Willand, 1916.)
YTTRIUM GLYCOLATE Y(C2H3O3)3.2H2O.
One liter of water dissolves 2.447 gms- of the salt at 20°.
(Jantsch and GrUnkraut, 1912-1913.)
YTTRIUM IODATE Y(IO3)3.3H2O.
100 gms. H2O dissolve 0.53 gm. yttrium iodate. (Berlin.)
YTTRIUM MALONATE Y2(C3H2O4)3.8H2O.
SOLUBILITY IN AQUEOUS MALONIC ACID AND AMMONIUM MALONATE
SOLUTIONS.
(Holmberg, 1907.)
Gms. YjCCsH/jO^j
Solvent. t°. per 100 Gms.
Solvent.
1 Gm. Am. Malonate per 10 cc. Solution 20 0.3
2 Gms. Malonic Acid per 10 cc. Solution 20 2.3
Gms. Yb2(S04)3
t°. per TOO gms. t.
H20.
Gms. Yb2(S04)3
per 100 Gms.
H20.
O
15-5
44.2
34-6
55
60
10-4
35
19.1
70
7 .22
747
YTTRIUM NITRATE
YTTRIUM Basic NITRATE 3Y2O3.4N2O5.2H2O.
EQUILIBRIUM IN THE SYSTEM YTTRIUM NITRATE, YTTRIUM, HYDROXIDE
AND WATER AT 25°. (James and Pratt, 1910.)
The determinations were made with very great care. The mixtures were ro-
tated 4^ months.
Sat. Sol. '
Gms. per 100 Gms
H2O.
Solid Phase. g^5 gol
Gms. per 100 Gms.
H?0.
•s Solid Phase.
Y(NO3)3.
Y203 as
Y(OH)3.
Y(N03)3.
Y203 as
Y(OH),.
1.0260
3-13
0
014
Y(OH)3 1.4867
73
•03
0.078
3Y203
4N206.2H20
.1106
13.87
o
034
"
.5587
89
.06
0
074
"
.1907
24.94
o
063
"
.6259
103
.80
0
075
"
•2517
33-02
0
160
"+3Y203.4N205.2H20
.6931
122
.40
o
080
«
-3268
44-35
0
114
3Y203.4N205.2H20
.7440
137
.IO
o
083
" +y(N03)3
.4104
58.61
0
095
"
.7446
141
.6
o
1
f(NQOs
YTTRIUM OXALATE Y2(C2O4)3.9H2O.
One liter H2O dissolves o.ooi gm. Y2(C2O4)s at 25°, determined by the elec-
trolytic method. (Rimbach and Schubert, 1909.)
100 gms. aqueous ammonium oxalate solution (3.26% (NH4)2C2O4.H2O)
dissolve 0.01714 gm. Y2(C2O4)3.9H2O at room temp. (Cleve, 1902.)
loo gms. aq. 2.16 n H2SO4 dissolve 0.6884 gm. Y2(C2O4)3 at 25°. (Wirth, 1912.)
loo gms. aq. 4.32 n H2SO4 dissolve 1.4 gms. Y2(C2O4)3 at 25°.
100 cc. aq. 20% methylamine oxalate dissolve 0.877 gm. yttrium oxalate at
ord. temp.
loo cc. aq. 20% ethylamine oxalate dissolve 1.653 gms. yttrium oxalate at ord.
temp.
100 cc. aq. 20% triethylamine oxalate dissolve 1.006 gms. yttrium oxalate at
ord. temp. (Grant and James, 1917.)
YTTRIUM Potassium OXALATE Y2(C204)3.4K2C2O4.i2H2O.
SOLUBILITY IN WATER AT 25°. (Pratt and James, 1911.)
The determinations were made with great care. The mixtures were constantly
rotated for 8 weeks.
^5 of Gms. per 100 Gms.
H2O.
Solid Phase.
Sol. ^
^(CA),
K2C204.
.008
Trace
1.31 Solid Solution
•035
O.O2
5-30
•059
O.O6
8.88
.096
0.27
14.50
.132
0.72
20.27
.166
i-37
26 . 02 Y2(C2O4)3.4K2C2O4.i2H2O
^5 Of Gms. per 100 Gms.
Sat. H2O.
Solid Phase.
Sol. Y2(CA)i. K,CA-
.174
.50 27 . 44 YJ(C204)3.4K2C2O4.i2H2O
.199
. 222
•49 32-83
.48 37-68
K
.231
.42 39.12
K2Q04
.228
.09 38.77
.218 o 37.87
"
YTTRIUM DimethylPHOSPHATE Y2[(CH3)2PO4]6.
100 gms. H2O dissolve 2.8 gms. Y2[(CH3)2PO4]6 at 25° and 0.55 gm. at 95°.
(Morgan and James, 1914.)
YTTRIUM SULFATE Y2(SO4)3.
SOLUBILITY OF YTTRIUM SULFATE IN AQUEOUS SOLUTIONS OF SODIUM
SULFATE AT 25°. (James and Holden, 1913.)
Equilibrium was reached very slowly and it was necessary to rotate the mixtures
for 14 months before final equilibrium was reached.
Gms. per 100 Gms.
H20.
Y2(S04)3.
Na2S04. '
5-6i
1.29
6.38
3-85
7.40
6.21
8.43
8.53
5-86
7-57
4-75
7.72
3-42
10.14
2.36
11.36
2.02
13.42
Solid Phase.
Y2(S04),
" +Y2(S04)3.Na2S04.2H20
Y2(SO4)3.NaiSO4.2H2O
Gms. per 100 Gms.
H20.
Y2(S04)3.
Na2S04.
1.90
14.89
1.79
16.51
1.86
18.44
2.99
19.96
3-°4
21.05
2.27
27.14
i-52
28.22
1.61
28.13
5.38
o
Solid Phase.
Y2(SO4)s.Na2SO4.2HsO
YTTRIUM SULFONATES 748
SOLUBILITY OF YTTRIUM SULFONATES IN WATER.
Gms. Anhy.
Sulfonate. Formula. t°. S^°Inc^te Authority.
Gms. H2O.
Yttrium Benzene Sulfonate Y(C6HSSO3)3.9H2O 15 60.4 (Holmberg, 1907.)
" m Nitro-
benzene Sulfonate Y(C6H4.NO3.SOs)3.7H2O 15 48.3
Yttrium Bromonitrobenzene
Sulfonate Y(C6H3Br.NO2.SO3.i.4.2)3.ioH2O 25 3.88 (Katz& James, '13.)
YTTRIUM TARTRATE Y2(C4H4O6)3.5H2O.
SOLUBILITY IN AQUEOUS TARTARIC ACID AND AMMONIUM TARTRATE
SOLUTIONS AT 2O0. (Holmberg, 1907.)
Gms. Gms.
Aq. Solvent. pe^Gms. Aq. Solvent. J£g£Ji
Sat. Sol. Sat. Sol.
1 gm. Am. Tartrate per 10 cc. 2 gms. Tartaric Acid per 10 cc.
solution 0.6 solution 0.02
2 gms. Am. Tartrate per 10 cc. i . i 4 gms. Tartaric Acid per 10 cc.
solution solution 0.02
ZEIN (Protein from Corn).
SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Galeotti and Giampalmo, 1908.)
Dry powdered zein was added to the alcohol + water mixtures and the solutions
kept at 25° and shaken frequently during 24 hrs. The removed undissolved resi-
due was dried to constant weight and weighed.
Vol. % CiHjOH" Gms. Zein per Vol. % Ci,H5OH Gms. Zein per
in Solvent. 100 Gms. Sat. Sol. in Solvent. 100 Gms. Sat. Sol.
10 0.05 60 18.57
20 O.II 70 I9-87
30 O.2I 80 7.8l
40 0.51 90 4.51
5O 1.43 IOO 0.02
Similar results are given for the solubility of zein in mixtures of C2H6OH + H2O
+ CHC13 at 20° and C2H5OH + H2O + acetone at 25°.
ZINC ACETATE Zn(C2H3O2)2.2H2O.
SOLUBILITY IN AQUEOUS ETHYL ALCOHOL AT 25°. (Seideii, 1910.)
TTT. m • Gms. Zn- W4. m Gms. Zn-
rHOTT ^ of (C2H302)2.2H2O rn'oH 4» of (C2H3O2)22H2O
£&S, Sat. Sol. per zoo Gms. Jt&SS Sat. Sol. per 100 Gms.
in Solvent. ^Sat Sd in Solvent. * Sat Sol
o .168 30.80 60 0.920 10. 60
10 .127 27.20 70 0.880 7.80
20 .090 23.70 80 0.850 5.50
30 .055 20.40 90 0.830 4.20
40 .015 17 95 0.825 4
50 0.970 13.80 loo 0.796 1.18*
* = gms. anhydrous salt. The solid phase was Zn(C2H3O2)2.2H2O in all cases except this solution.
ioo gms. H2O dissolve 41.6 gms. Zn(C2H3O2)2.H2O at 15°, d of sat. sol. = 1.165.
(Greenish and Smith, 1902.)
ioo cc. anhydrous hydrazine dissolve 4 gms. zinc acetate with separation of a
white suspension at ordinary temperature. (Welsh and Broderson, 1915.)
ZINC ARSENATE Zn3(AsO4)2.8H2O.
ioo gms. 95% formic acid dissolve 0.26 gm. Zn3(As04)2 at 21°. (Aschan, 1913.)
ZINC ARSENITE Zn3(AsO3)2.
ioo gms. 95% formic acid dissolve 0.36 gm. Zn3(AsO3)2 at 21°. (Aschan, 1913.)
749 ZINC BENZOATE
ZINC BENZOATE Zn(C7H6Oa)a.
SOLUBILITY IN WATER.
(Pajetta, 1906.)
t°. 15-9°. 17°. 27-8°. 31-3°. 37-5°. 49-8°. 59-°
Cms. Zn(C7H5O2)2 per
100 gms. aq. solution 2.55 2.49 2.41 2.05 1.87 1.62 1.45
ZINC BROMIDE ZnBr2.2H2O.
SOLUBILITY IN WATER.
(Dietz, 1900; see also Etard, 1894.)
t°.
Gms. ZnBrg
per too Gms.
Solution.
Mols. ZnBr2
per TOO
Mols.H20.
Solid
Phase.
t°.
Gms. ZnBr2
per 100 Gms.
Solution.
Mols. ZnBr3
per 100
Mols.H2O.
Solid
Phase.
-T5
77-^3
27.0
ZnBr2.3H2O
25
82.46
37-6
ZnBr2.2H2O
— 10
78-45
29.1
"
30
84.08
42-3
«
- 5
80.64
33-3
"
37
86.20
50.0
"
- 8
79.06
30.2
ZnBr2.2H2O
35
85-45
46.9
ZnBra
o
79-55
31-1
"
40
85-53
47-4
"
+ 13
80.76
33-5
"
60
86.08
49-5
"
18
81.46
35-i
"
80
86.57
5I-S
M
100
87.05
53-8
M
ZINC BICARBONATE Zn(HCO3)2.
SOLUBILITY OF ZINC BICARBONATE IN WATER CONTAINING CARBON DIOXIDE.
(Smith, 1918.)
For description of the experimental method see iron bicarbonate, p. 336.
Results at 25°. Results at 30°.
Atmospheres
Pressure of
C02, Calc. by
Henry's Law.
Gm. Mols.
Free H2CO3
per Liter.
Gm. Mols.
Zn(HCO3)2
per Liter.
Gm. Mols.
Free H2CO3
per Liter.
Gm. Mols.
Zn(HC03)2
per Liter.
4.12
0.1390
0.00194
0.1838
O.OO2I5
5-33
0.1797
O.OO2II
0.3838
0.00277
7.64
0.2579
0.00242
0.4038
0.00286
10.61
0.3580
O.OO27O
0.4601
o . 00308
12. 16
0.4103
0.00278
o . 6064
0.00324
13.29
o . 4480
O.OO29I
0.6257
0.00337
19-73
0.6657
0.00317
0.7470
0.00352
20.65
0.6969
0.00319
0.8351
0.00376
22.56
0.7610
0.00343
I . 0840
0.00339
40.61
I.370I
0.00445
I.I275
0.00429
The calculated pressures are lower than the actual pressures since Henry's Law
does not hold at very high pressures.
" If zinc carbonate were not hydrolytically dissociated, its solubility in pure
water at 25°, would be 4.58 X io~* gms. mols. per liter." (Smith, 1918.)
ZINC CARBONATE ZnC03.
Ageno and Valla (1911) report that the solubility of ZnCO3 in water at 25° is
1.64. io~4 mols. = 0.206 gm. per liter.
One liter of aq. 5.85% NaCl solution dissolves 0.0586 gm. ZnCO3 at 14°.
One liter of aq. 745% NaCl solution dissolves 0.0477 gm. ZnCO3 at 14°.
(Cantoni and Passamanik, 1905.)
ZINC CHLORATE
750
ZINC CHLORATE ZnClO3.
SOLUBILITY IN WATER.
(Meusser, 1902; at 18°, Mylius and Funk, 1897.)
-18
o
8
15
18
Cms.
Zn(ClO3)2
too Cms. per 100
Mols.
Zn(C
per
Solution.
55-62
59-19
60.20
67.32
66.52
Solid Phase.
H20.
9 . 70 Zn(ClO3)2.6H2O
II.08
11.72
15.96
15.39 Zn(C103)2.4H20 —13
Sp. Gr. of solution saturated at 18° = 1.916.
Cms. Mols.
Zn(C103)2 Zn(C103)2 Solid Phase
per 100 Cms. per 100 Mols. " ^nase.
Ice
Solution.
30 67.66
4O 69 . 06
H20.
16.20
17.29
55 75-44
Ice curve
24
13 30.27
9 26.54
3-36
2.80
ZINC CHLORIDE ZnCl2.
SOLUBILITY IN WATER.
(Mylius and Dietz, 1905; see also Dietz, 1900; Etard, 1894.)
A0 Gms.ZnCl2per looGms. Solid
Gms.ZnCkper looGms. Solid
Water. Solution. Phase.
' Water.
Solution.
Phase.
- 5
14
12.3 Ice
9
360
78.3
.aiH2O + .H2O
— 10
25
20- o
6
385
79-4
ZnCl2.2iH2O
-40
83
45-3
6
298
74-9
ZnCljj.iJHjjO
-62
104
51.0 Ice + Zn£I2.4H20
10
330
76.8
"
-5o
"3
53.0 ZnCl2.4H2O
20
368
78.6
•«
-40
127
55-9
26
423
80.9
.i}H20+ZnCl2.H2O
-30
1 60
6l-5 ^H20 + .3H20
26.3
433
81.2
.iJH2O + ZnCla
-10
189
65.4 ZnCl2.3H2O
0
342
77-4
ZnCl2.H2O
o
208
67.5
10
364
78.4
"
+ 5
230
69.7
20
396
79.8
"
6-5
252.4
71.6
28
436
81.3
ZnCl2.H20 + ZnCla
5
282
73-8
31
477
82.7
ZnCl2JH2O
0
309
25
432
81.2
ZnCla
o
235
70 • I ZnCl2.2iH2O
.40
452
81.9
•«
6.5
252
71-6 .2}H2O + .3H2O
60
488
83.0
«
10
272
73 • * ZnCla-aiHaO
80
543
84.4
«
12.5
303
75.2
100
615
86.0
••
«•$
335
262
CO
IOO.O
«
SOLUBILITY OF OXYCHLORIDES OF ZINC IN AQUEOUS SOLUTIONS OF ZINC
CHLORIDE AT ROOM TEMPERATURE.
(Driot, 1910.)
ZnCl2.
ZnO.
ouiiu jriiase.
8.22
0.0137
ZnCl,.4ZnO.6H2O
23.24
0.138
"
45-95
0.497
"
51.5
0.604
"
56.9
0.723
«'
' ZnCl2.
ZnO. '
62.85
0.884
ZnCl2.4Zn0.6H20
96
1.792
"
124.7
3-213
"
144.8
2.64
"
203
i-59
ZnClj.Zn0.iiH2O
Results are also given for mixture of the oxychloride and oxide in aqueous zinc
chloride solutions at various temperatures.
751
ZINC CHLORIDE
SOLUBILITY OF ZINC CHLORIDE-AMMONIUM CHLORIDE MIXTURES IN WATER.
(Meerburg, 1903.)
Isotherm for o°.
Cms. per ioo Gms.
Solution. Solid
ZnCl2.
0
NH4C1.
22.8
NH4C1
3-5
23.0
"
7 -1
23-5
H
10.2
23-9
"
15-1
24.7
"
18.0
25-3
"
22.4
26.0
"
24.2
26.1
"
25-7
26.3
NH4C1 +
27-5
26.4
a
30-7
25-7
"
33-9
25-3
««
38.8
24.4
"
42.6
24.6
a + b
44-3
21-3
b
49-2
15 .3
"
52.6
11.9
"
55-4
IO.O
"
59-3
7-5
••
62.1
6.8
M
Isotherm for 20°.
Isotherm for 30°.
Gms. per ioo Gms.
Solution.
ZnCl2.
NH4C1. '
o.o
26.9
5-i
27.1
9-5
27.4
12.7
27-5
J5-7
27.7
18.0
27.9
23-5
29.0
26.0
29-5
29-5
28.1
32-3
27.7
35-8
27.0
38-7
26.9
40.2
26.6
41.9
26-3
43-2
26.0
46.9
21 .O
53-2
14-5
58-4
II .1
62 .7
8.7
66.6
7-9
Solid
Phase.
NHiCl
Gms. per ioo Gms.
Solution.
NH4C1 + .
a
a + b
b
ZnCI2.
NH4C1.
0-0
29-5
9.2
29.4
16.0
29.7
2O. 2
30.1
24.7
30-4
26.3
30.8
27.2
30.2
30.1
29.6
36.8
28.2
42.4
27-3
43-8
27-3
45-o
24.4
5r-2
I7.6
61 .9
10-4
66.9
9-2
75-6
6.1
7o-3
7.6
78.5
3-2
76.9
3-5
79-8
1.6
81.6
o.o
Solid
Phase.
NHiCl
ZnClj
a = ZnCl2.3NHCl3,. b =
IOO gms. abs. acetone dissolve 43.5 gms. ZnCl2 at 18°, d& of sat. sol. = 1.14.
(Naumann, 1904.)
ioo gms. glycerol dissolve 50 gms. ZnCl2 at 15.5°. (Ossendowski, 1907.)
loo cc. anhydrous hydrazine dissolve 8 gms. ZnCl2 at room temp.
(Welsh and Broderson, 1915.)
When I gm. of zinc as chloride is dissolved in ioo cc. of aq. 10% HC1 and
shaken with ioo cc. of ether, 0.03 per cent of the metal enters the ethereal layer.
(Mylius, 1911.)
ZINC CHROMATES.
EQUILIBRIUM IN THE SYSTEM ZINC OXIDE, CHROMIUM TRIOXIDE AND
WATER AT 25°.
(Groger, 1911.)
An excess of ZnO was, in each case, shaken for 3 days at 25°, with gradually in-
creasing concentrations of chromic acid.
Gms. per Liter Sat. Sol.
Solid Phase.
Gms. per Liter Sat. Sol.
ZnO.
Cr03. '
0.409
0.604 4ZnO.CrO3.3H2O
2.24
4.19 "
5- .86
II.5 " +3ZnO.CrO3.2H2O
10.7
22.2 3ZnO.CrO3.2H2O
26.7
57-5 "
30-4
66.7 " +4ZnO.CrO3.3H2O
32.2
70 . 6 4ZnO.CrO3.3H2O
ZnO.
66.1
CrO3.
151
ouuu jruase.
4ZnO.CrO3.3H2O
83.7
123
192
285
" +3Zn0.2Cr03.H20
3ZnO.2CrO3.H2O
193
196
450
46l
" +ZnO.CrO3.H2O
202
389
475
940
ZnO.CrO3.H20
ZINC CINNAMATE 752
ZINC CINNAMATE Zn(C6H6CH:CHCOO)2.
100 cc. sat. solution in water contain 0.144 §m« zmc cinnamate at 26.5°.
(De Jong, 1909.)
ZINC CYANIDE Zn(CN)2.
100 cc. concentrated Zn(C2H3O2)2 + Aq. dissolve 0.4 gm. Zn(CN)2.
100 cc. concentrated ZnSO4 -j- Aq. dissolve 0.2 gm. (Joannis, 1882.)
loo gms. H2O dissolve 0.24 gm. zinc mercuric thiocyanate, ZnHg(CNS)4at 15°.
(Robertson, P. W., 1907.)
ZINC FLUORIDE ZnF2.4H2O.
One liter of water dissolves 16 gms. at 18°.
(Dietz, 1900.)
ZINC HYDROXIDE Zn(OH)2.
One liter of water dissolves 0.0042 gm. ZnO at 18°, conductivity method.
(Dupre and Bialas, 1903.)
One liter of water dissolves o.oi gm. at 25°. (Bodlander, 1898.)
SOLUBILITY OF ZINC HYDROXIDE IN AQUEOUS SOLUTIONS OF:
Ammonia and Ammonia Bases at I7°-I9°.
(Herz, 1902.)
Sodium Hydroxide at Ord. Temp.
(Rubenbauer, 1902.)
Normality
of
Normality
of Dis-
Gms. ZnO
Gms. per 20 cc. Solution _ MoL
the Base.
solved Zn.
Solution.
Na. Zn. the NaOH.
0.0942NH3
O-OOII
0.00185
0.1012 0-0040 4 .50
0.236 "
O.OIIO
O.OlSo
0.1978 O.OI5O 2.33
0.707 "
0.059
0.0958
0.4278 O.O442 I .06
O.O005
O-OOoS
0-6670 O.I77I 0.70
0.472
O-OoSl
0.0132
0.9660 0.9630 0.48
0.944
O.O3
0.0484
1.4951 0.2481 0.31
0.068 NH2C2H5
0.0003
0.0005
2.9901 0.3700 0.16
0.51
O.0045
O.OO74
Moist Zn (OH) 2 used. So-
0.68
0-0098
0-0161
lutions shaken 5 hours.
SOLUBILITY OF ZINC HYDROXIDE IN AQUEOUS SOLUTIONS OF AMMONIUM
HYDROXIDE.
Results of Euler (1903).
Results of Bonsdorff (1904) at 25°.
t°.
Normality
of Aq.
Ammonia.
Mols. Zn
per Liter.
Normality
of Aq.
Ammonia.
Gms. ZnO
per Liter.
Normality
of Aq.
Ammonia.
Gms. ZnO
per Liter.
15-17
0.485
O.OI3-O.OIO*
0.3II
0.85
0.321
0-34
15-17
0.97
0.034
0.825
3-84
0.643
0.845
21
0-253
O.OO29
1.287
7.28
I.2I5
2.70
21
0.259
0.0022*
1.928
5-07
21
0.500
O.OO97
2.570
7.01
21
0.518
O.OO7O
3-213
10. 16
f Euler states that the higher results of Herz are due to incompletely purified
zinc hydroxide and uses material precipitated from the nitrate for his experiments.
Different preparations of Zn(OH)2 containing from 55 to 77 per cent H2O were
used and in the two cases marked * ZnO was used.
Bonsdorff used for his second series of determinations, Zn(OH)2 precipitated
from the nitrate and brought in moist condition into the ammonia solutions.
753 ZINC HYDROXIDE
SOLUBILITY OF ZINC HYDROXIDE IN AQUEOUS POTASSIUM HYDROXIDE
SOLUTIONS.
(Klein, 1912.)
The determinations were made by adding aq. ZnSO4 solution (containing one
gm. mol. per liter) to aq. KOH solutions until a permanent precipitate just
appeared. The titrations are also recalculated to mols. per liter and correction
made for the dilution of the KOH solution by the aq. ZnSO4.
Normality of
Aq. KOH.
cc. ZnSO4
Sol. per 50 cc.
Aq. KOH.
t^aicu
tacea iviois. per i^uer 01
oat. aoi.
Oric Cone.
KOH.
Corrected Cone,
of KOH.
Cone, of Zn.
I
5-5
t
0.9
O.IO
1.78
13-1
I.78
1.42
0.209
2
14-3
2
I.S6
0.223
2.22
17.9
2.22
1-63
0.266
2-5
18.8
2-5
I.8l
0.272
3
24.6
3
2.02
0.330
3-6
29.1
3-6
2.28
0.368
4
34
4
2.38
0.405
6
56 (?)
6
2.78
0.540
SOLUBILITY OF ZINC HYDROXIDE IN ONE PER CENT AQUEOUS SALT
SOLUTIONS AT i6°-2o°.
(Snyder, 1878.)
The CO2 free Zn(OH)2 dissolved is calculated as milligrams Zn per liter of the
given salt solution. Additional determinations are also given.
Aq. Salt Mgs. Zn per Aq. Salt Mgs. Zn per Aq. Salt Mgs. Zn per
Solution. Liter Solution. Solution. Liter Solution. Solution. Liter Solution.
Nad 51 K2S04 37.5 K2C03 o
KC1 43 MgS04 27 NH4C1 95
CaCl2 57.5 KN03 17.5 NH4N03 77
MgCl2 65 Ba(N03)2 25 (NH4)2S04 88
BaCl3 38
ZINC IODATE Zn(IOi)i.
100 gins. H2O dissolve 0.87 gm. Zn(IO3)2 cold and 1.31 gms. hot.
(Rammelsberg, 1838.)
ZINC IODIDE ZnI2.
•
SOLUBILITY IN WATER.
(Dietz, 1900; see also Etard, 1894.)
Gms. ZnI2 Mols. ZnI2 Gms. ZnI2 Mols. ZnI2
t°. per 100 Gms. per 100 Solid Phase. t°. per 100 Gms. per 100 Mols. Solid Phase.
Solution. Mols.H2O. Solution. H2O.
— IO 80.50 23.3 ZnI2.2H2O O 8l.II 24.2 ZnI3
— 5 80.77 23-7 " *8 81.20 24.4 "
o 81.16 24.3 " 40 81.66 25.1 "
+ 10 82.06 25.8 " 60 82.37 2^-4
22 83.12 27.8 " 80 83.05 27.5
27 89.52 50.3 " TOO 83.62 28.7
Sp. Gr. of sat. solution of the anhydrous salt at 18° = 2.725.
loo gms. glycerol dissolve 40 gms. ZnI2 at 15.5°. (Ossendowski, 1907.)
ZINC
NITRATE
754
ZINC
NITRATE
Zn(N03)2.
SOLUBILITY IN WATER.
(Funk, 1900.)
Gms.
Mols.
Gms.
Mols.
*
Zn(NO3)oper ZnNO3 per Solid
* • TOO Gms. 100 Phase.
t °.
Zn(N03)2per
100 Gms.
Zn(N03)2
100
per Solid
Phase.
Solution.
Mols. H2O.
Solution.
Mols. H20.
-25
40.12
6.36
Zn(NO3)2.9H2O
18
53-50
IO-9
Zn(N03)3.6H20
— 22
•5 40-75
6-54
44
25
55-90
12 -O
44
— 20
42.03
6.89
M
36-4
63.63
I6.7
"
-18
43-59
7-34
"
36
64.63
17.4
41
-18
44-63
7.67
Zn(NO3)2.6H2O 33.5 65 . 83
I8.3
44
~~I5
45.26
7.86
it
37
66.38
z8.«
Zn(N03)2.3H20
-13
45-51
7-94
*
40
67.42
19.7
««
— 12
45-75
8.01
(i
4i
68.21
20.4
M
0
48.66
9.01
41
43
69.26
21.4
44
-1-12
•5 52-0
10,3
•4
45-5
77-77
33-3
M
ZINC OXALATE ZnC2O4.2H2O.
One liter H2O dissolves 0.0057 Sm- ZnC2O4 at 9.76°, 0.0064 §m- at I7-92° and
O.OO7I5 gm. at 26.15°. (Kohlrausch, 1908.)
SOLUBILITY OF ZINC OXALATE IN AQUEOUS AMMONIUM OXALATE
SOLUTIONS AT 25°.
(Kunschert, 1904.)
Mol. Normal (NH4)2C204
Mol. Zn per Liter
0.05 o.io 0.15 0.20 0.25
0.0022 0.0055 °-OIO55 0.0174 0.0257
Complex ammonia zinc oxalates are formed. When more than 0.15 free oxalate
is present the complex has the formula, (NH4)4Zn(C2O4)3. In the more dilute
solutions it has the composition, (NH4)2Zn(C2O4)2.
ZINC Ammonium PHOSPHATE ZnNH4PO4.
One liter sat. solution in water contains 0.0136 gm. ZnNH4PO4 at 10.5° and
0.0145 gm. at 17.5°. (Artmann, 1915.)
ZINC SULFATE ZnSO4.
SOLUBILITY IN WATER.
(Cohen, 1900; at 50°; Callender and Barnes, 1897; Etard, 1894; Poggiale, 1843; Mulder.)
t°.
Gms. ZnSO4
per 100 Gms. Solid «. o
Solution.
Water.
Phase.
- 5
28.21
39-30
ZnSO4.7H2O 25
O.I
29-54
41-93
39
9.1
32.01
47-09
" 5°
IS
33-81
50.88
70
25
36.67
57-90
80
35
39-98
66.61
90
39
41 .21
70.05
100
- 5
32.00
47-oS
ZnSO4.6H2O 1 2O
01
33-09
49.48
140
1 60
ns. ZnSO4
per 100 Gms
Solid
Phase.
Solution.
Water.
38-94
63.74
ZnSO4.6H2O
41 .22
70.06
.6H2O + .?H2O
43-45
76.84
ZnS04.6H20
47-5
88.7
.6H20 + .H2O
46.4
86.6
ZnSOvHzO
45-5
83-7
44
44-7
80.8
44
41 .7
71 .5
44
38.0
61-3
44
33-o
49-3
44
TheSp. Gr. of a sat. sol. of ZnSO4 in water at 15° is 1.452. (Greenish and Smith, i
Data for the solubility of ZnSO4 in water at high pressures are given by Cc
and Sinnige (1909, 1910.)
902.)
Cohen
755
ZINC SULFATE
SOLUBILITY OF ZINC SULFATE — SODIUM SULFATE MIXTURES IN WATER.
(Koppel, Gumpery, 1905.)
Gms. per 100
Gms. Solution.
Gms. per 100
Gms H2O.
Mols.
Mols.
3er 100
H2O. Solid
t °.
ZnSO4.
Na2SO4
ZnSO4. Na2SO4. ZnSO4.
Na2S04: Phase'
o
27
.19
5
•33
40.30
7.90
4
•50
I
. OI ( ZnSO4.7H2O +
5
27
•85
6
.27
42.28
9-52
4
•71
1
2 j j Na2SO4.ioH2O
25
17
•58
15
•63
26.32
23.40
2
•94
2
.96 ZnNa2(SO4)2.4H2O
30
17
.66
15
•58
26.47
23-44
2
•95
2
•97
35
17
•59
15
.70
26.36
23-52
2
•94
2
.98
40
17
•75
15
•72
26.68
23-63
2
.98
2
•99
10
29
.16
7
.16
45-79
ii .24
5
.11
I
.42 •
15
30
.70
6
.40
48.81
10.17
5
•45
I
.29
20
25
32
•Si
5
4
•36
.41
52-34
56-15
8.62
7.22
6
.84
•27
I
O
.09
.91
3o
36
^28
3
.80
60-55
6-34
6
.76
0.8l
35
38
.18
3
•30
65-25
5-64
7
.28
O
.71 J
38
40
38
38
•83
.26
2
2
.90
.78
66.64
64.89
4.98
4.71
7
7
•44
.24
0
0
•63
.60
10
27
.91
7
.92
43-50
12.34
4
•85
I
•565
20
24
19
.28
.14
10.90
14.58
36.92
28.77
16.71
21.95
4
3
.12
.21
2
2
.12
•79
25
13
•31
19
•94
J9-93
29.87
2
.22
3
•785
30
6
.96
27
•75
10.67
42-51
I
.19
5
•39 J
35
5
.61
30
•03
8.72
46.61
O
.971
5
.91
ZnNa2(SO4)24H2O
40
5
.96
28
•65
9.16
43-83
I
.02
5
•555 .
"7~N<l2SO4
SOLUBILITY OF ZINC SULFATE IN AQUEOUS ETHYL ALCOHOL.
(Schiff, 1861.)
Concentration of Alcohol 10 per cent
Gms. ZnSO4.7H2O per 100 Gms. Solution 51.1
20 per cent 40 per cent
39 3-45
100 gms. abs. methyl alcohol dissolve 0.65 gm. ZnSO4 at 18°, 5.90 gms.
ZnSO4.7H2O at 18°.
100 gms. 50 per cent methyl alcohol dissolve 15.7 gms. ZnSO.7H2O at 18°.
(de Bruyn, 1892.)
100 gms. glycerol dissolve 35 gms. zinc sulfate at 15.5°. (Ossendowski, 1907.)
ZINC SULFIDE ZnS.
One liter H2O dissolves 70.6. lO"6 mols. ZnS = 0.0069 Sm- at l8°. determined
by the conductivity method, assuming complete dissociation and hydrolysis.
(Weigel, 1906, 1907.)
ZINC SULFITE ZnSO3.2H2O.
IOO gms. H2O dissolve 0.16 gm. ZnSO3.2H2O. (Houston and Trichborne, 1890.)
ZINC SULFONATES
SOLUBILITY IN WATER.
Formula.
Gms. Anhy.
Name. Formula. t°. Salt per 100 Authority.
Gms. H20.
Zinc |8 Naphthalene Sulfonate (CioH7.S03)2Zn.6H2O 25 0.45 (Witt, 1915.)
Zinc 2-Phenanthrene " (Ci4H9.S03)2Zn.6H2O 20 0.083 (Sandquist, '12.)
3- " " (Ci4H9.S03)2Zn.4H2O 20 0.19
20 0.15
ZINC SULFONATES
756
SOLUBILITY OF ZINC PHENOLSULFONATE, p (C6H4.OH.SO3)2Zn.8H2O, IN
AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1910.)
Wt.%C_ .
in Solvent.
O
20
40
47
60
<*25 Of
Sat. Sol.
1.185
1. 161
1. 106
GmS. (CgH4.OH.- »rr. c/ /-• TT /~VTT
cr» \ v., str f) n~, VVt. % C2H5Uil
t Sol in Solvent-
39-8
40.7
42.1
42.2
41.6
80
90
92.3
95
IOO
4.5 Of
Sat. Sol.
1-057
1.047
1.048
1.052
J-o75
Gms. (C6H4.OH.-
S03)^Zn.8H20 per
40.7
41.4
41.9
42.9
ioo gms. H2O dissolve 37 gms. (C6H4.OH.SO3)2Zn.8H2O at 15° and di5 of sat.
sol. = I.I62. (Greenish and Smith, 1902.)
ZINC TARTRATE C4H4O6.Zn.2H2O.
SOLUBILITY IN WATER.
(Cantoni and Zachoder, 1905.)
15
20
25
30
35
Gms.
C4H4O6.Zn.2H2pper
ioo cc. Solution.
0.019
0.022
0.036
0.041
°-°55
40
45
50
55
60
Gms.
n^Hjp per
ioo cc. Solution.
0.060
0.073
0.087
0.116
0.104
65
70
75
80
85
Gms.
C4H4O6.Zn.2H2O per
ioo cc. Solution.
o.ioo
0.088
0.078
0.059
0.041
ZINC VALERATE Zn(C4H9COO)2.2H2O.
SOLUBILITY OF ZINC VALERATE IN AQUEOUS ALCOHOL SOLUTIONS AT 25°.
(Seidell, 1910.)
Wt. %
C2H5OH
in Solvent.
^5 Of
Sat. Sol.
Gms. Zn(C4H9-
COO)2.2H2O
per ioo Gms.
Sat. Sol.
Wt.%
C2H5OH
in Solvent.
d25 of
Sat. Sol.
Gms. Zn(C4H9-
COO)2.2H20
per ioo Gms.
Sat. Sol.
0
1.004
1.44
85
0.836
2-15
20
0.972
0-75
90
0.827
3-20
40
0.936
0.76
92-3
0.828
5-50
00
0.894
I-I5
95
0.832
8.80
80
0.848
1.70
IOO
0.844
15.60
ZIRCONIUM SULFATE Zr(SO4)2.
SOLUBILITY OF ZIRCONIUM SULFATE IN AQUEOUS SULFURIC ACID AT 37.5°.
(Hauser, 1907.)
Gms. per ioo Gms. Sat. Sol.
ZrO2.
S03.
19-5
25.46
18.8
27
16.2
29.1
9-6
32.3
5-3
34.7
3-51
36.01
1.03
38.2
0.46
39-8
0-33
42.1
o. 14
46.8
Gms. per ioo Gms. Sat. Sol.
•
Zr(S04)2.4H20
ZrO2.
SO3.
0.15
56.7
0.50
57-5
2
59-5
4-4
61.4
4-55
61-5
3-33
63.8
i. 80
64.2
I. 12
66.8
0.96
68.4
0.10
81.5
+Zr(S04)2.H2S04.3H20
Zr(so,)2.Haso4.3H,o
Zr(S04)2.H2SO4.H2O
Results at 22° show only slight differences from the above figures, hence, the
temperature coefficient for this salt is quite small. In an earlier paper Hauser
(J905) gives data for the basic sulfate 4ZrO2.3SO3.i4H2O.
METHODS FOR THE DETERMINATION OF
SOLUBILITY
A quantitative determination of a solubility consists essentially
of two operations; the preparation of the saturated solution and its
subsequent analysis. In those cases where these steps are per-
formed separately the method may, in general, be designated as
the analytical and in those where they are combined, as the syn-
thetic. In both cases, however, the consideration of first import-
ance is the assurance that final equilibrium between solvent and
solute has been reached. Since this point is that at which no further
change occurs in the relation between the amount of the compound
in solution and that remaining undissolved, the only criterion of
saturation is the evidence that the concentration of the solution has
not changed during a longer or shorter interval of time, during
which those conditions which would tend to promote such a change
have been allowed to operate.
Of the conditions which promote most effectively the attainment
of equilibrium between a solute and a solvent, the provision for the
intimate contact of the two is most important. In other words,
only by the thorough mixing which agitation or effective stirring
provides can the point of saturation be reached with certainty. In
the case of the reciprocal solubility of liquids, the point of equi-
librium is usually attained within a much shorter period than in the
case of solids dissolved in liquids. In the latter case, the necessary
disintegration of the solid, incident to its solution in the liquid, is a
process which is restricted to the surface layers of the solid, and,
therefore, unless a large area, such as a finely divided state provides,
is available, and unless that portion of the solvent which has acted
upon a given surface area is repeatedly replaced by fresh solvent,
the process of solution will be greatly retarded. It is quite evident
that, although a solution in contact with even very finely divided
solid may promptly become saturated in the immediate vicinity of
the solid without stirring, the distribution of the dissolved material
to the remainder of the solvent would depend upon diffusion, and
since the rate at which this proceeds would diminish as the concen-
tration differences became equalized, the process would take place
757
METHODS FOR THE DETERMINATION OF SOLUBILITY
at a gradually diminishing rate. If the point of equilibrium is
approached from supersaturation, the above remarks apply with
equal effect, since only at the surface of the solid can the excess of
salt leave the solution and, without other provision than diffusion
for successively bringing the entire amount of the solution in con-
tact with the solid, the deposition of the excess of dissolved material
can occur only at a very slow rate. The importance of active and
continuous agitation of the solid and solution, in effecting satura-
tion, cannot, therefore, be too strongly emphasized. It may in fact
be assumed that determinations of the solubility of solids, made
without continuous agitation, are always open to the suspicion that
the results do not represent the final equilibrium which soich data
are required to show.
Since solubility is a function of temperature, the accurate control
of the temperature in making a solubility determination is another
one of the indispensible requisites of accuracy. In general, it may
be stated therefore, that every procedure designed for preparing a
saturated solution must include provision for the accurate control
of the temperature and for active and continuous agitation or stir-
ring of the solution. In the case of the solubility of gases, which will
be considered in a separate section, provision for the control of the
pressure must also be made.
It is obvious that since the solubilities of various compounds
differ, and that of one compound is affected by the presence of an-
other, the accurate determination of this constant for a particular
molecular species presupposes that only this one substance is pres-
ent in the pure solvent. That is, accuracy of results demand that
only pure compounds be involved in a given determination, con-
sequently, no effort should be spared to make it certain that the
highest possible purity of both solute and solvent has been attained.
Apparatus for the Determination of the Solubility of Solids by the
Analytical Method. — The types of apparatus which have been
developed for the preparation of saturated solutions of solids in
liquids differ principally in respect to whether designed for multiple
or single determinations at a given temperature. Examples of the
first type are illustrated by Figs. I and 2.
It will be noted that in the one case (Fig. i) the bottles containing
the solutions are stationary and the liquid in each and in the con-
stant temperature bath is kept in motion by means of revolving
stirrers. This form of apparatus was used by Moody and Leyson
(1908) for the determination of the solubility of lime in water and is
particularly adapted for relatively slightly soluble compounds for
758
METHODS FOR THE DETERMINATION OF SOLUBILITY
FIG, i.
METHODS FOR THE DETERMINATION OF SOLUBILITY
which rather large quantities of the saturated solution are needed
for accurate analysis. There is also shown in the figure the pro-
vision for withdrawing the saturated solution through a filter
within the inverted thistle tube. The stirrers in the bottles are
fitted with mercury seals to prevent access of air containing carbon
dioxide. Other features of the apparatus will be readily understood
from the drawing.
A more common type of apparatus, designed for the simultaneous
saturation of several solutions at the same temperature, is that
illustrated by Fig. 2, in which the bottles containing the solutions
are slowly rotated in the constant temperature bath. The form
shown is that described by Noyes (1892). This type of apparatus
has the advantage that the solid is, to a large extent, kept in suspen-
sion in the liquid and, therefore, offers the most favorable oppor-
tunity for continuous and uniform contact with the solution. Many
examples of this form of apparatus, differing principally in size and
in the direction of movement of the containers, are described in the
literature.
Of the second type of apparatus, designed for a single determina-
tion at a given temperature, many varieties have been developed
for particular conditions. Of these, the following examples have
been selected as typical of this class and, it is hoped, will illustrate
most of their desirable features. They are, in general, adaptations
of earlier designs and it is not intended that the name given in con-
nection with each is that of the investigator who deserves the credit
for originating the type. The drawings will, for the most part,
be readily understood without detailed explanations. The dimen-
sions are not stated, since they can usually be varied to suit the
needs of almost any problem.
In Fig. 3 is shown the apparatus used by the Earl of Berkeley
(1904) for the very careful determinations of the solubility of
inorganic salts in water. The features of particular interest in
connection with it are, that the water bath itself is made to serve
as the temperature regulating device, and the apparatus for with-
drawing and simultaneously filtering the saturated solution is a
combination of pipet and pycnometer. This was provided with
ground glass caps for each end and the stem was accurately grad-
uated. It was, of course, carefully standardized before use. The
flexible iron plate shown was made of a disc from the receiver of
a telephone. The apparatus was used for determinations at tem-
peratures between 30° and 90° and the range of variations from
the set temperature of the bath was, for 2-3 hour periods, within
760
METHODS FOR THE DETERMINATION OF SOLUBILITY
about 0.2°. For the inner vessel containing the salt, the range
was about 0.05°. At each temperature two determinations of den-
sity and solubility were mad ; one on the solution obtained by
stirring a supersaturated solution in contact with solid salt, and
the other on the solution obtained by stirring an unsaturated solu-
tion in contact with an excess of salt.
FIG. 3.
In the case of determinations at the boiling point a special
apparatus was required. Two forms, described by the Earl of
Berkeley (1904), are shown in Figs. 4 -and 5. The first was used
for the less soluble salts and consisted of an outer tube A con-
taining water and an inner tube B containing salt and solution.
By boiling the water vigorously and closing the side tube C, steam
passing through the tube D stirred the solution thoroughly and
the temperature rose to the boiling point of the saturated solution
and remained constant when saturation was attained. The second
form of apparatus (Fig. 5) was devised for use with extremely
761
METHODS FOR THE DETERMINATION OF SOLUBILITY
soluble salts. In these cases it was found that the larger quan-
tity of steam required for thorough stirring dissolved so much
salt that it was necessary to have a very large excess present. In
this apparatus the steam was generated in a boiler A and conducted
through the tube B to the bottom of the large test tube C containing
the excess of salt and solution. The test tube was immersed in the oil
THERMOMETER
PLWINUM HIRE.
FOR PULLING OFF
THE FILTER —
THERMOMETERS
PLATINUM
WIRE FOR
PUL UNG OFF
f/LTEK
STIRRER
FIG. 4.
FIG. 5.
bath D which was vigorously stirred and maintained at a tempera-
ture close to that of the boiling point of the saturated solution.
When the temperature of the oil bath was below the boiling point,
salt dissolved; when above, salt was thrown out of solution.
Considerable difficulty was experienced in filling the pycnometer
with the saturated solution without introducing errors due to
steam bubbles caused by the suction which was applied.
762
METHODS FOR THE DETERMINATION OF SOLUBILITY
A comparatively simple form of the type of apparatus used by
Victor Meyer in 1875 and modified by Reicher and van Deventer
(1890) and by Goldschmidt (1895), is described by Hicks (1915) and
shown in the accompanying Fig. 6. A glass cylinder A is closed at
FIG. 6.
FIG. 7.
each end with large one-hole rubber stoppers. The mixture of salt
and solution is contained in this cylinder and is stirred by the
rotation of the tube E which is provided with an enlargement at
its lower end in which there are two small holes at H and I. The
763
METHODS FOR THE DETERMINATION OF SOLUBILITY
stirrer rotates in the bearing formed by the hollow wooden cylin-
der J. The glass rod K carries a rubber stopper L which closes
the filtering tube M, in which a platinum cone N supports an
asbestos filter 0. The siphon P connects the filtering tube with
the flask R which is provided with an outlet through the small
tube S. The apparatus is immersed in a constant temperature
water bath W, to about the level shown After stirring the mix-
ture of salt and solution a sufficient length of time for attainment
of saturation, the undissolved salt is allowed to settle and the
rubber stopper is withdrawn from the filter tube by means of the
glass rod K. Suction is applied through the tube 5 to hasten
the filtering and the clear solution collected, at the temperature of
the bath, in the previously weighed flask R.
A similar apparatus was used by Walton and Judd (1911), for
determination of the solubility of lead nitrate in pyridine. This
is shown in Fig. 7 and consists of a glass test tube fitted with a
stirrer which turns in a mercury seal, thus preventing loss of
solvent by evaporation or the admission of moisture from the air.
To take a sample of the saturated solution, the weighing tube A
was introduced into the larger tube through a hole in the stopper.
After reaching the temperature of the bath the stirrer was stopped,
the end of the small tube B, which was covered with a piece of
closely- woven muslin, was dipped below the surface of the solu-
tion and the liquid drawn into A by applying suction at C. The
tube A was then removed, weighed and the contents analyzed.
An apparatus which was used by Donnan and White (1911),
for the determination of equilibrium in the system palmitic acid
and sodium palmitate is shown in Fig. 8. The stirring in this case
was accomplished by means of a current of dry air, free of carbon
dioxide. The apparatus consists of two parts, namely, an inner
chamber E, where equilibrium was attained, and an outer case A,
designed for isothermal filtration. The whole was immersed in a
thermostat to the level W. A side tube B permitted connection
with a filter pump. C is a weighing bottle to receive the filtered
saturated solution and D a Gooch crucible provided with a paper
filter. The cork, closing A, was covered with a plastic layer to
render it air-tight. The tube at the lower end of E was closed
with a ground glass plug F, the stem of which was enlarged to a
small bulb at G and then drawn out to pass easily through H,
leaving an air free outlet around it. The small cork I was used
to support the stopper when lifted to allow the contents of E to
flow down for filtration. The dry air by which the mixture was
764
METHODS FOR THE DETERMINATION OF SOLUBILITY
stirred was drawn through K by applying suction at H. The
preheating of this air was accomplished by drawing it through a
thin spiral immersed in the thermostat. The connection between
the equilibrium apparatus and preheater was made through a
mercury seal, which permitted lifting the apparatus easily without
damage to the fragile preheater permanently mounted in the
bath. This apparatus provided for the recovery, separately, of
FIG. 8.
the saturated solution and undissolved solid. These authors also
describe an improved electrically heated and controlled constant
temperature bath.
Determinations at lower temperatures than can be constantly
maintained with the aid of a water bath require special forms of
apparatus which permit of temperature control under more or
less restricted conditions. An apparatus of this type, which was
used by Cohen and Inouye (1910), for determination of the solu-
bility of phosphorus in carbon disulfide, is shown in Fig. 9, and
is intended for the range of temperature between — 10° and +10°.
The saturating vessel D consists of a glass cylinder to the upper
765
METHODS FOR THE DETERMINATION OF SOLUBILITY
end of which is cemented a steel collar E, containing a deep channel.
A mixture of litharge and glycerol was used as the cementing
material for this purpose. The inverted steel cover F fits into the
channel of this collar and the seal of the joint is effected, in the
usual way, by means of a layer of mercury. The cover F is pro-
vided with a brass tube K, to which the pulley M is attached, and
FIG. 9.
is also pierced by the tightly cemented-in glass tube /. The glass
rod Gt containing on its lower end the three stirring wings H H H,
is cemented into the brass tube K. The saturating vessel is, for
stability, tightly fastened in a hole in a block of lead, 5, contained
in the Dewar cylinder A. An atmosphere of CO2 in the saturat-
ing vessel is provided by introducing CO2 under pressure through
7 and allowing the excess to escape through the mercury seal in E.
After charging the apparatus, / is closed with a rubber tube and
plug and the stirrers H H H set in motion. A Witt stirrer, O,
keeps the contents of the bath in rapid circulation. Water is
766
METHODS FOR THE DETERMINATION OF SOLUBILITY
used in the bath for temperatures above o°, and alcohol for those
below o°. The regulation of the temperature is accomplished by
addition of ice or solid CO2 as found necessary and, therefore, re-
quires very close attention on the part of the experimenter.
A novel and simple form of apparatus, which was used by Bahr
(1911), for the determination of the solubility of thallium hydroxide
at temperatures up to 40° is shown in Fig. 10. As will be seen, this
FIG. ii.
consists of a gas washing flask to the arms of which a Y tube pro-
vided with two stop-cocks is sealed. The inside walls of the
apparatus were coated with hard paraffin and the required amounts
of thallium hydroxide and water introduced. It was then im-
mersed in a water bath and the contents stirred by means of a
current of hydrogen, which entered as shown and with A and E
closed, passed through D and out at B. When it was desired to
767
METHODS FOR THE DETERMINATION OF SOLUBILITY
remove a sample of the solution for analysis, B and D were closed
and the liquid forced through A into the pycnometer by means of
gas pressure entering through E. For temperatures above 40°,
the form of apparatus shown in Fig. n was used. In this case K
represents a copper cylinder with double walls, of which the inner
compartment G, contains concentrated salt solution which is
stirred by a stream of air (not shown), and the outer compart-
ment contains a layer of heating liquid H. The glass tube L con-
tains the mixture of thallium hydroxide and water which is stirred
by means of a current of hydrogen (not shown). When saturation
is attained the tube A , of small bore and thick walls and provided
with a small asbestos filter, is introduced and the saturated solution
forced over into the receptacle B by pressure of hydrogen which
enters at C. The heating liquid in B is the same as used in H.
The following heating liquids with the boiling points shown were
used: Allyl chloride, 46°; Ethylene chloride, 55°; Chloroform, 61°;
Methyl alcohol, 66°; Benzene, 80°; Benzene-Toluene mixture, 91°;
Water, 100°.
A somewhat more elaborate apparatus, in which the constant
temperature is maintained by means of the vapor of a boiling
liquid, is shown in Fig. 12. This apparatus was developed by
Tyrer (1910) for the very accurate determination of the solubili-
ties of anthraquinone, anthracene and phenanthraquinone in single
and mixed organic solvents. The solvent with excess of the solute
was placed in A and kept in constant agitation by means of the
vertically acting stirrer shown. The tube A is surrounded by a
bath of vapor which circulates through the cylinder B, condenses
in C, and returns to the boiling flask M. When the solution is
saturated it is allowed to settle, and the clear solution run out
(by raising the tube D) into a small graduated flask E, which is
maintained at the same temperature as the solution A. The tem-
perature of the vapor bath is varied by changing the pressure
under which the liquid in the- flask M is boiling. For this purpose,
the manostat P is provided. The temperature can, with care, be
maintained constant to 0.01°. For this purpose the apparatus
must be air-tight, the liquid in the boiling flask must not bump
(which is entirely prevented by placing a layer of mercury in the
flask) and a pure boiling liquid must be used.
Although illustrations of special forms of apparatus designed for
securing equilibrium in solubility determinations could be extended
far beyond the number given, it is believed that the principal
features have been made clear and it will no doubt be possible to
768
METHODS FOR THE DETERMINATION OF SOLUBILITY
adapt the devices here shown to many other cases for which accu-
rate determinations of solubility may be desired.
Separation of Saturated Solution from Undissohed Solid. — The
next point, after the establishment of equilibrium between the
FIG. 12.
solvent and solution, is the matter of successfully separating the
saturated solution from the undissolved solid, preparatory to its
analysis. There are, undoubtedly, many cases where this is a very
serious problem. This is especially so for extremely soluble com-
pounds, which yield viscous solutions as well as for those which
do not readily settle out of the solution or cannot be removed by
769.
METHODS FOR THE DETERMINATION OF SOLUBILITY
ordinary filtration. It is, of course, necessary to maintain the
mixture at the temperature at which saturation was obtained until
the complete separation of the solution and solid has been effected.
The operation should, therefore, as a general thing, be conducted
in the same bath used for preparing the saturated solution. Sev-
eral forms of apparatus designed for this purpose are shown in
the diagrams given in the preceding pages. For solutions which
can be readily separated from the undissolved solid, a graduated
pipet to which a stem with a plug of filtering material can be
attached and which is adapted to being easily weighed, is the most
convenient.
Analysis of the Saturated Solution. — The weight of a known
volume of the perfectly clear solution, that is, its specific gravity,
should always be determined. This weighed quantity of solution,
or a known dilution of it, furnishes a very convenient sample for
the determination of the amount of dissolved compound.
In regard to the analysis, the procedure must be selected en-
tirely on the basis of the number and character of the constituents
present. In cases of the solubility of single non-volatile compounds,
in solvents which can be more or less easily removed by volatiliza-
tion, the plan in most general use is the evaporation of a known
amount of the solution to dryness and weighing the residue. Special
forms of apparatus to be used for this purpose have been proposed
from time to time. These are, usually, vessels with tubular open-
ings, arranged so that a current of dry air can be drawn over the
surface of the heated sample.
In the case of solubility determinations in which the saturated
solution contains more than one dissolved compound, the applica-
tion of the usual gravimetric or volumetric procedures will, of
course, be necessary. Where unique methods have been developed,
a brief reference to them will usually be found in the body of the
book, in connection with the results for the compound in question.
In certain cases, where the direct determination of the amount
of the dissolved compound present in the solution would be very
difficult or impossible, an indirect method can sometimes be used.
For this purpose, a carefully weighed amount of the compound
must be used, and, after the period of saturation, the undissolved
residue is filtered off under conditions which reduce losses to a
minimum and, after drying to its original condition, it is weighed,
and the amount which has been dissolved found by subtracting
the weight of the undissolved residue from the quantity originally
present.
770
METHODS FOR THE DETERMINATION OF SOLUBILITY
Identification of the Solid Phase. — As already mentioned in the
chapter on General Information, the solubility of a compound,
which is capable of existing in several forms, depends upon the
particular form in which it is present in contact with the satu-
rated solution. The question of the composition of the solid phase
is, therefore, of considerable importance for the accurate deter-
mination of solubility. Although the identification of the solid
phase presents little difficulty in the majority of cases, it some-
times happens that it can be made only by a more or less indirect
method. The principal reason for this is that adhering solution can
usually not be completely removed from the solid phase and the
analysis, consequently, does not give direct information of the
required accuracy.
A method which has been used considerably for identifying the
solid phase is that known as the residue method of Schreinemakers
(1893). It is based on the principal that if an analysis is made of
both the saturated solution and of a mixture of the saturated solu-
tion and the solid phase of unknown composition, the two points so
obtained, when plotted on a coordinate system, lie on a line con-
necting the point representing the composition of the solid phase and
the solubility curve of the system. Similar analyses of another sat-
urated solution of the system and of its mixture with the solid
phase, locate another such line. Since all lines so determined
when extended, pass through the point representing the compo-
sition of the solid phase, their intersection locates this point
definitely.
Although the original description of this method by Schreine-
makers was illustrated by an example drawn on the rectangular
system of coordinates, it has been used much more extensively, in a
practical way, in connection with the later developed equilateral
triangular diagram. In this case, each apex of the triangle repre-
sents one of the three components of the system, each point on a leg,
a mixture of two, and each point within the triangle a mixture of all
three components. When a number of saturated solutions are
analyzed, the results correspond to points on the solubility curve of
the system. If now some of the solid phase with adhering solution
is removed from each mixture and analyzed, it is evident that the
results thus obtained, being for samples made up of both the satu-
rated solution and the solid phase, give points which lie on lines
connecting the two. The points on the curve for the pure saturated
solutions being known, it is necessary only to connect them with the
points for the corresponding mixtures of solid phase and saturated
771
METHODS FOR THE DETERMINATION X)F SOLUBILITY
solution, and to prolong the lines to their common intersection.
This will necessarily be at the point representing the composition
of the pure solid phase.
In applying the residue method of Schreinemakers, if the inter-
secting lines which fix the point corresponding to the solid phase
meet at a very narrow angle, definite information as to its composi-
tion may not be secured. For cases such as these, a procedure to
which the name "tell-tale" method was given by Kenrick (1908)
and which is described in detail by Cameron and Bell (1910), has
been developed. This method consists in adding to the mixture a
small amount of an entirely different compound which remains
wholly in the solution. After equilibrium has been reached, a por-
tion of the saturated solution and of the solid phase with adhering
solution are analyzed, and the quantity of the added "tell-tale"
compound in each determined. From the result, showing the con-
centration of the added compound in the saturated solution, and the
amount of it found in the mixture of solid and solution, the quantity
of solution in contact with the solid can be calculated. Since the
composition of the solution is also known, the difference between
the composition of the solid plus solution and of the amount of
solution known to be present, is the composition of the pure solid.
Transition Temperatures can frequently be accurately determined
by relatively simple means, and since such data are useful in estab-
lishing fixed points on solubility curves they are valuable adjuncts
to directly determined solubility data.
Synthetic Method. — The procedures which have, so far, been
mentioned are all classed as analytical methods of solubility deter-
mination. In contradistinction to these is the equally useful reverse
process, by which the solvent and solute are brought together' in
previously measured quantities and the temperature ascertained at
which the solution is saturated. To this procedure the designation
synthetic method of solubility determination has been applied.
One of the earliest investigators to use this method extensively was
Alexejeff (1886) and it is, therefore, frequently referred to as the
Alexejeff synthetic method of solubility determination.
The synthetic method can, of course, be used both for the solu-
bility of solids in liquids and for liquids in liquids, but it is in the
latter case that it is of greatest service. Its points of superiority,
particularly in the case of the reciprocal solubility of liquids, are
that the upper limits of the determinations can be extended far
beyond the boiling point temperature and are, in fact, limited only
by the resistance of the glass to pressure or to the action of the
772
METHODS FOR THE DETERMINATION OF SOLUBILITY
liquid. Only small quantities of the solute and solvent are required
for a determination. It is applicable to compounds for which
quantitative methods of analysis are not available or are of a tedious
character. The mixtures, being contained in sealed tubes, are not
subject to the action of constituents of the air, nor are losses, due to
volatilization, to be feared. Although, in the case of solids, diffi-
culties incident to the supersaturation, resulting from failure of the
crystals to separate on cooling, are encountered, with liquids
the point of saturation is made instantly and strikingly evident by
the beginning of opalescence or clouding which occurs, and errors
due to supersaturation are rarely encountered. A sure criterion
that supersaturation does not occur rests on the observation of the
temperature at which the cloudy solution again clears. If this
temperature coincides with the temperature of the beginning of
opalescence, it is certain that supersaturation has not occurred.
The observation of the temperature of saturation can be repeated
as often as desired, and the accuracy of the determination is ordi-
narily limited only by the care taken in making it.
The limitations of the method, aside from the supersaturation
which may occur in the case of solids, are principally those resulting
from the low temperature coefficients of solubility possessed by
certain compounds, and which usually occur in the vicinity of
maxima or minima of solubility curves. Although a "critical cloud-
ing" occurs in the vicinity of the so-called critical solution point,
this possesses a characteristic appearance which is easily distinguish-
able from the clouding observed at the saturation point, and errors
of observation due to it are not to be apprehended. In fact, it has
been pointed out that supersaturation disappears at the critical
point, and the synthetic method is ordinarily very accurate in the
vicinity of the critical solution temperature.
Since, by the synthetic method the results are necessarily obtained
under different pressures, this question has been given consideration
from the theoretical and the practical side. Although it is possible
that extremely high pressures would exert an influence, the conclu-
sion appears justified, that under ordinary conditions, in which
pressures of 10 atmospheres are not exceeded, no notable effect
would be produced. The solubility curves obtained by this method
do not show any abnormalities due to this cause.
In the case of the determination of the solubility of solids by the
synthetic method, the operation consists in preparing a mixture of a
carefully determined amount of the solvent and of the solid, and
subjecting it to gradually increasing temperature and to constant
773
METHODS FOR THE DETERMINATION OF SOLUBILITY
agitation, while a continual observation of the changes taking place
in the solid is made. When all but a few small crystals have dis-
solved, the change in temperature is regulated much more carefully
and note is taken of the point at which the edges of these final
crystals begin to change from sharp to rounded, or vice versa, or
where the sizes of the particles visibly increase or diminish. Care
must, of course, be taken not to allow the last portions of the solid
to dissolve; otherwise, on cooling, considerable supersaturation may
occur before the solid begins to separate from solution. The method
is, naturally, most serviceable where the change in solubility with
temperature is considerable, and where convenient methods for the
direct analysis of the solution are not available.
The procedure of a determination in the case of the reciprocal
solubility of liquids consists in introducing by means of capillary
funnels weighed amounts of the two liquids into small glass tubes
and sealing the ends. The amount of air space in the tubes should
be kept low. Many convenient devices for weighing and intro-
ducing the liquids have been described. In the case of very volatile
liquids it may be necessary to introduce them in thin walled bulbs,
which can be broken after the tube containing the mixture has been
sealed. The tube is then placed in a large beaker of water, or higher
boiling liquid if necessary, and heat applied until the contents of the
tube, on being shaken, become homogeneous. The^temperature is
then allowed to fall very slowly and an observation made, while the
tube is constantly agitated, of the temperature of first appearance
of opalescence. This observation can be repeated as many times as
desired and the temperatures of appearance and disappearance of
the clouding, which usually differ by only a few tenths of a degree,
can be ascertained with certainty.
Since, by the synthetic method the data are for irregular intervals
of temperature, in order to obtain results for a particular tem-
perature it is necessary to plot the several determinations on coordi-
nate paper and from the solubility curve so obtained, read the value
for the temperature in question.
Freezing-point Method. — A modification of the synthetic method,
which is applicable particularly to solutions which contain relatively
large amounts of the dissolved compound, is that which consists in a
determination of the freezing-point of the mixture. This point is,
in fact, the temperature at which the separating solid compound is
in equilibrium with the solution.
The difference between the freezing-point determination and the
observation of the point of growth or diminution of a crystal in a
774
METHODS FOR THE DETERMINATION OF SOLUBILITY
liquid is that, in the former, the establishment of equilibrium is
recognized exclusively by the change of the thermometer. The
solution is cooled gradually, during which the thermometer sinks
slowly to a point below the freezing temperature. As soon as the
first crystal appears, either spontaneously or by intentional intro-
duction (seeding), the thermometer rises suddenly to the freezing-
point and remains stationary for some time.
This method can, of course, be used in a large number of cases for
the determination of solubility. Those portions of the solubility
curves of salts in water for which ice is the solid phase, are practi-
cally always determined in this way and it may be said, in general,
that for determinations made at low temperatures, the freezing-point
method is to be selected whenever possible.
For the practical execution of the method the very well known
apparatus of Beckmann is most convenient and satisfactory. The
determinations must, of course, be made with all the refinements
which have been developed for accurate freezing-point measure-
ments.
The method has been used extensively for the discovery of
addition compounds. Its use for this purpose is based upon the
principle that if to a pure compound, A, a second, B, is added, the
freezing-point of A is lowered; similarly the freezing-point of B is
lowered by A, and the two descending curves thus obtained inter-
sect at the eutectic. If, however, a compound, AxBy is formed,
this also acts as a pure substance and its freezing-point is lowered
by either A or B. Hence the freezing-point lines do not meet at a
single eutectic but exhibit in this case a maximum, the position of
which indicates the composition of the compound.
Volume Change Method. — Still another method, which is a modi-
fication of the synthetic, is that designed to indicate the reciprocal
solubility of liquids by a determination of the volume changes which
occur when two relatively sparingly miscible liquids are shaken
together in a closed vessel. The apparatus consists usually of a
cylindrical receptacle which is provided with a constricted grad-
uated section either at one end or near the middle. Such volumes of
liquids are chosen that the meniscus separating them lies in the
constricted graduated tube. The determination consists in super-
imposing measured volumes of each liquid and noting the position
of the meniscus before and after a period of shaking at constant
temperature. From the increase or decrease of volume of the two
layers, as estimated from the change in position of the meniscus,
the reciprocal solubility of the two liquids is calculated. It is to be
775
METHODS FOR THE DETERMINATION OF SOLUBILITY
noted, however, that the solubility of liquids is in practically all
cases reciprocal, and without an analysis of the two layers the true
solubility can not usually be deduced.
Titmtion Method. — A special case of the reciprocal solubility of
liquids is that representing equilibrium in ternary systems yielding
two liquid layers. Such equilibria are usually determined by rel-
atively simple titration procedures, but for the interpretation and
description of the results, special terms have been developed and
these require more or less detailed explanation.
When a third liquid is added to a mixture of two others which are
miscible to only a slight extent,, the added liquid, if soluble in each
of the others, will distribute itself between the two and an equi-
librium will be reached. If the two layers are then analyzed and
the results plotted on coordinate paper, two points, corresponding
to the two layers, will be obtained. If more of the third liquid is
added, equilibrium will again be established after a short period of
shaking and the analysis of the two layers, to which the designation
conjugate layers has been given, will fix two more points when plotted
on the coordinate paper. The process may be repeated until a
considerable number of points have been obtained. When this has
been done, it will always be found that these points are the locus of a
smooth curve, to which the designation binodal curve has been given.
If the pairs of points corresponding to the conjugate layers are
connected, the lines so obtained are defined as tie lines. Since it is
evident that with the continued addition of the third or consolute
liquid, a point must finally be reached at which the resulting mixture
will no longer separate into two conjugate layers, the tie lines suc-
cessively determined as above described, will become shorter and
shorter until finally the last one is reduced to the point correspond-
ing to the homogeneous mixture of the three components. To this
is given the name plait point.
Although for the above example a ternary system made up of
three liquids has been taken, there are a large number of salts and
other solid compounds which, when dissolved in mixtures of liquids
of certain concentrations, cause the latter to separate into conjugate
liquid layers. These systems have aroused much interest from time
to time and considerable data for them are given in the literature.
Since it is usually difficult and frequently impossible to analyze
directly a homogeneous mixture of liquids, and thus determine the
points on a binodal curve, a simple titration method for this purpose
has come into general use. By means of this a homogeneous
mixture of known amounts of two of the components is titrated with
METHODS FOR THE DETERMINATION OF SOLUBILITY
the third just to the point of initial separation of the second
layer, which is usually very sharply indicated by the appearance of
clouding or opalescence. The procedure may also be reversed and
the consolute liquid added just to the point of clearing of the cloudy
mixture of the other two. By this plan the synthetically derived
composition of one of the two conjugate layers and thus of one point
on the binodal curve is known. The determination of the tie line
and therefore, the identification of the corresponding point on the
curve for the conjugate liquid, requires an additional experiment
for its location. Several procedures for this purpose have been de-
veloped. They usually depend upon the determination of one or
more constants of specially prepared pairs of conjugated liquids,
such as their specific gravities or refractive indices. In the case
of mixtures of which one member can be easily determined analyti-
cally, tie lines can be located by the quantitative determination of
this member in pairs of conjugated liquids.
In general, the titration method for the determination of the
solubility of liquids is applicable to many cases. The facts, that
equilibrium is attained so promptly in liquids and that the evidence
of the appearance of a second insoluble layer is usually so striking,
make it of great value. Refinements have been introduced such
as the addition of liquid or solid dyes to the mixture in order to
facilitate the detection of the end point, and the development of
particular forms of apparatus for measuring and weighing the
liquids. The constituents of the mixtures are usually weighed but
the volume relations and, therefore, the specific gravities can also
be approximately estimated, by using graduated vessels for making
the titrations, and measuring in them the volumes of the final
mixtures. A very ingenious method for ascertaining indirectly the
composition of the liquid mixtures in the case of the system
naphthalene, acetone and water, is described on p. 444.
As a usual thing the temperature coefficients are not very great
in the case of liquid mixtures and the very accurate control of the
temperature is not imperative. When such control is necessary,
however, the use of a thermostat does not seriously complicate the
determination.
Distribution Coefficients. — As mentioned above, when a third
compound is added to a mixture of two liquids which are relatively
immiscible, it will dissolve to a certain extent in each and the com-
position of the two layers represent conjugate points on the binodal
curve for the system. The results are, however, of interest from
another point of view, namely that of the distribution of the com-
777
METHODS FOR THE DETERMINATION OF SOLUBILITY
pound between the two solvents. This distribution coefficient is,
in many cases, of considerable interest in connection with analytical
methods based on shaking out procedures and also in connection
with such problems as the molecular state of compounds in solution,
their dissociation and other points of theoretical interest. Distri-
bution coefficients have, therefore, been studied to a large extent
and much data for them are available. In general, the determina-
tions are made by relatively simple methods. The amount of the
compound present in a definite amount of each layer, after equi-
librium has been established by adequate agitation, is determined
in any manner most convenient. If the total amount of solute is
known, and that found in one layer, the amount in the other can, of
course, be calculated by difference. The results are usually ex-
pressed on the volume basis, since it is the ratio of the amounts
present in the same molecular state in equal volumes of the two
layers which is a constant, independent of temperature and con-
centration.
It is evident that when the concentration at the saturation point
is considered, the amount of the compound which enters each layer
depends upon its solubility in the liquid, consequently the dis-
tribution coefficient is the relation of the solubilities of the dissolved
substance in the two solvents. Variations from this, aside from
changes in molecular state, etc., in one or the other solvent are due
to such causes as the reciprocal solubility of the so-called immiscible
solvents, which will, of course, be influenced by the presence of the
dissolved compound, especially at the higher concentrations. Vari-
ations of the coefficient with temperature would result in cases
where the solubilities of the compound in the two solvents do not
change at the same rate with temperature.
Electrolytic Conductivity Method. — Of the physical properties
which can be used for the determination of the concentration of a
solution, such as specific gravity, refractive index, etc., the electro-
lytic conductivity is of particular value in the case of those very
sparingly soluble compounds which yield solutions too dilute to be
analyzed by gravimetric or volumetric methods. By its use the
progress of the saturation can be followed without separating the
undissolved solid from the solution, or even removing the portion
used for the determination. The special electrical equipment
which is required, however, and the need for water of exceptional
purity and of vessels of particular qualities, restrict its general use.
The method of calculating the concentration from the conduc-
tivity is based on the assumption that at the very great dilutions
778
METHODS FOR THE DETERMINATION OF SOLUBILITY
involved, complete dissociation occurs. Therefore, the limiting
value to which the equivalent conductivity approaches at infinite
dilution is, for practical purposes, attained, and A = A*> = la + /*,
where la and 4 are the ionic conductivities of the anions and kations.
These values are known for all the principally occurring ions. The
observed specific conductivity K is, however, connected with the
equivalent conductivity and the concentration t\ by the equation
A = -, in which 77 represents the concentration in gram-equivalents
V
per cubic centimeter. Rearrangement and substitution give
TJ = j — r— T- . From this equation the solubility of the substance
I'a T i'k
under investigation is calculated by substituting the measured
specific conductivity of the solution and the known values of the
ionic conductivities.
The Solubility of Gases in Liquids. — When a gas and a liquid are
intimately mixed by shaking, a definite amount of the gas will be
dissolved by the liquid and, simultaneously, the vapor of the liquid
will mix with the gas in the space above the liquid. The partial
pressure of the liquid in the gas space is almost exactly the same as
that of the pure liquid at the solution temperature, since the in-
fluence of the relatively slight amount of dissolved gas is insignifi-
cant in by far the most cases. The amount of gas which is dissolved
depends both on the nature of the gas and of the liquid and is,
furthermore, a function of the temperature, and pressure.
In regard to the influence of pressure, the absorption law of Henry
holds for the most part, when the gas solubility is not too great.
According to it, the amount of pure gas, which is taken up at con-
stant temperature by a given amount of liquid is proportional to
the pressure of the gas.
The temperature acts almost always in the sense that the solu-
bility decreases as the temperature rises.
The solubilities of gases are usually expressed either in terms of
the Bunsen "Absorption Coefficient" /3, or the Ostwald "Solubility
Expression" /. Definitions of these are given on p. 227.
The experimental methods for the determination of the solubility
of gases vary according to the nature of the gas. For those which
dissolve in relatively large amounts and can be analytically deter-
mined with accuracy, the saturated solution may be analyzed by
ordinary quantitative methods. Thus, in the case of the solubility
of sulfur dioxide in aqueous solutions of salts (see p. 706, results by
Fox, 1902), the solutions were saturated by passing a stream of the
779
METHODS FOR THE DETERMINATION OF SOLUBILITY
gas through them at atmospheric pressure and, when equilibrium
was attained, a measured portion of the solution was withdrawn,
transferred to an excess of standardized iodine solution and the
excess of the latter titrated with thiosulfate. A gravimetric pro-
cedure was used by Christoff (1905) for the determination of the
solubility of carbon dioxide in aqueous salt solutions. In this case
the solutions were weighed before and after the passage of the gas
through them and the increase in weight, after applying necessary
corrections, taken to represent the solubility at the temperature of
the experiment and at atmospheric pressure. The absorption flasks
were of special shape and the gas was previously passed through a
series of U tubes, containing the same aqueous solution, in order
to prevent loss of water from the experimental solution which,
otherwise, would have occurred.
In the great majority of cases, however, gas solubility is deter-
mined by a method based upon the measurement of the volume of
the gas absorbed. The apparatus consists essentially of an absorp-
tion flask for the liquid, connected by means of a tube of small bore
to a graduated buret in which the gas is measured above mercury,
the level of which can be altered by raising or lowering a container
connected with the buret by means of a rubber tube. Many forms
of this apparatus have been described and the disadvantages of the
earlier forms have gradually been remedied. A relatively simple
form of this apparatus, but one which embodies the essential
features required for accuracy, is that described by McDaniel (1911)
for the determination of the solubility of methane, ethane and
ethylene in a large number of organic solvents at various tem-
peratures.
This apparatus is shown in Fig. 13. A is an ordinary gas buret
and B an absorption pipet of the form first used by Ostwald. "The
buret and pipet are connected by means of the glass capillary M
sealed directly onto each, so that the whole forms one solid piece
of glass apparatus without rubber or cement connections of any kind;
thus any possibility of leaks from these extremely troublesome
sources is entirely avoided. The whole apparatus is clamped
solidly to a rigid support so that it can be taken up in the hands
and shaken for the purpose of bringing the gas into intimate contact
with the liquid. The pipet and buret are each provided with a
three-way stopcock, C and D. These can be turned in such a way
as to allow the gas to sweep out the air from the connecting capillary.
By the same means the two vessels may also be connected directly
with each other as well as separately with the outside air or source
IETHODS FOR THE DETERMINATION OF SOLUBILITY
of gas supply. The pipet and buret are each provided with a water
jacket, P and Q. The temperature of each is regulated by means
of the electrically heated coils K and L." These coils are of
manganin wire and are connected in series. The rate of evolution
of heat in the jackets was adjusted in the first place by varying the
length of the manganin wire, until the temperature was the same in
each jacket. Stirring was accomplished by blowing air through
the tubes I and /. The differences in temperature between the
pipet and buret were never greater than 0.1°.
T
M
B
FIG. 13.
FIG. 14.
In carrying out a determination by this method it is, of course,
necessary that the solvent be completely free of dissolved air or
other gas. This is perhaps the most important part of the deter-
mination and a special form of apparatus for the purpose is described
by McDaniel (1911) and is shown in Fig. 14. "The liquid was
boiled under diminished pressure in the flask C attached directly
781
METHODS FOR THE DETERMINATION OF SOLUBILITY
to the lower opening of the pipet by means of the rubber stopper as
shown in the figure. Connection with the air pump is made at D.
During the boiling the lower opening of the inlet tube E is above the
surface of the liquid in C, the stopcock B being closed. When the
air has been completely expelled, the screw pinchcock F is closed
while the air pump is still in operation. The flask C is now raised
until the lower end of E reaches nearly to the bottom of the flask.
The air pump is now connected at G and the cock H opened so as
to make connection with the pipet. B is now opened and the inflow
of air through D regulated by gradually opening F in such a manner
that the liquid is very slowly forced up into the pipet. In this
manner the liquid never comes into contact with the air under full
atmospheric pressure but only under greatly diminished pressure.
The absorption of air under these conditions can only be inappre-
ciable, especially since the liquid in the flask remains perfectly quiet,
and only the lower portion is used."
Having filled the pipet B, Fig. 13, with the air-free solvent as
just described, "T is connected with the source of gas supply and
the cocks C and D are turned in such a way as to allow the gas to
sweep out the air from the capillary, M. The buret is then filled
in the usual manner by lowering the leveling tube F, the cock D
having been turned so as to connect T with E. Care is taken to
keep the entering gas under a slight pressure by keeping the mercury
level in F slightly above that in A . This prevents air from entering
through any leaks in the train connecting the gas generator with the
buret." The gas must be completely saturated with the vapor of
the solvent and this, with other than aqueous solvents, may require,
in addition to drawing it through some of the solvent in H, that a
thin layer be placed in the buret and time allowed for it to saturate
the gas sample.
"After again allowing the current of gas to flow through the
capillary M for a short time the buret and pipet are connected with
each other by turning the three-way cocks D and C in the proper
direction. The determination of the amount of absorption is then
made as follows: A portion of the gas is passed into the pipet by
raising F and opening G, the displaced liquid being caught in a
graduated cylinder. The cock C is closed and the gas and liquid in
the pipet brought into intimate contact with each other by shaking
the whole apparatus. C is now opened to allow gas to enter from
the buret to replace that absorbed. This process is repeated until,
on opening C, there is no further decrease in the volume of gas in A.
The volume absorbed is found by subtracting from the original
782
METHODS FOR THE DETERMINATION OF SOLUBILITY
volume of gas, the volume remaining in the buret plus the volume
in the pipet. The volume of gas in the pipet is equal to the volume
of liquid drawn off. The volume of liquid remaining is easily
calculated from the known volume of the pipet. The absorption
coefficient or ' solubility ' is the ratio of the volume of gas absorbed ,
measured at the temperature of the experiment, to the volume of
the saturated liquid. It may be reduced to the coefficient used by
Bunsen by dividing by (i + a/)."
In the case of the majority of investigators who have used this
method, particularly for determinations at high or low tempera-
tures, the absorption pipet has been kept at the temperature of the
experiment and the gas measuring buret at room temperature, the
two being connected by means of a flexible capillary which permits
the absorption pipet to be independently shaken. This arrange-
ment makes it necessary, in calculating the absorption coefficients,
to apply the usual corrections for temperature and vapor pressure
to the volume of gas in the buret. This is a complication which in
some cases causes uncertainties in regard to the accuracy of the
results as finally calculated.
A somewhat more elaborate form of apparatus than that just
described was developed by Drucker and Moles (1910) for determi-
nations in cases where the solubility is very small. These authors
give results for hydrogen and nitrogen in aqueous solutions of
glycerol. The particular feature of the apparatus is that only about
one-tenth the usual amount of solvent is employed and solubilities
as low as only one-tenth that of nitrogen in water at 25° can be
measured.
An apparatus designed for determinations at very high pressures,
using a Caillet compression tube, is described by Sander (1911-12).
It was used for determination of the solubility of carbon dioxide in
water, alcohols, and other organic solvents. The principle involved
TS that the pure gas is first compressed above mercury in a graduated
tube and the volumes corresponding to given pressures noted. Simi-
lar readings are then taken for the same gas after a small accurately
measured amount of solvent has been introduced into the graduated
tube. The difference between the two volumes at the same tem-
perature and pressure, reduced to I kg. per sq. cm. and I cc. of
liquid, represents the solubility of the gas in the given solvent.
Finally, attention should be called to the method of determination
of gas solubility based on the principle that, for volatile solutes
which obey the laws of Dalton and Henry, the amount which is
carried away by an inert gas when known volumes are bubbled
783
METHODS FOR THE DETERMINATION OF SOLUBILITY
through solutions of known strength of volatile solute, can be used
to measure the comparative solubilities in solvents of different con-
centrations. An example of this method is the determination of
the solubility of ammonia in aqueous salt solutions by Abegg and
Riesenfeld (1902). The very ingenious apparatus consists of a
generator for developing a stream of H2 + O2 from aqueous NaOH,
by means of an electric current measured with the aid of a copper
voltmeter, and the volume of gas thus determined. This was passed
through a spiral in the vessel containing the ammonia solution of
known concentration. The mixed gases passing out of this were
received in a third vessel containing 5 cc. of o.oi n HC1. Electrodes
were provided in this' vessel and, by means of conductivity measure-
ments, the point determined at which all of the HC1 became satu-
rated with NH3. Since the volume of the H2 + O2 required for this
purpose was known, the partial pressure of the NH.s in the mixture
could be directly ascertained. Comparative determinations of the
vapor pressure of the ammonia in water and a series of salt solutions
made in this way were calculated to ammonia solubilities on the
basis of the relation that, for two solutions of equal ammonia con-
tent, the ammonia pressure is reciprocally proportional to the solu-
bility of the ammonia in them.
784
AUTHOR INDEX
Abbott, G. A. and Bray, W. C.
(1909) J.Am.Chem.Soc., 31, 729-763-
Abe, Ryuji.
(1911) Mem.Coll.Sci.Eng. (Kyoto),
3, 212.
(1911) J.Tok.Chem.Soc., 32, 980.
(1911-12) Mem.Coll.Sci.Eng.
(Kyoto), 3, 13.
(1912) J.Tok.Chem.Soc., 33, 1087.
Abegg, R.
(1903) Z.Elektrochem., 9, 550.
Abegg, R. and Cox, A. J.
(1903) Z.physik.Chem., 46, n.
Abegg, R. and Pick, H.
(1905) Ber., 38, 2573.
(1906) Z.anorg.Chem., 51, I.
Abegg, R. and Riesenfeld, H.
(1902) Z.physik.Chem., 40, 84.
Abegg, R. and Sherrill, M. S.
Z.Elektrochem., 9, 550.
Abegg, R. and Spencer.
(1905) Z.anorg.Chem., 46, 406.
Acree, S. F. and Slagle, E. A.
(1909) Am.Chem.Jour., 42, 135.
Adrian!, J. H.
(1900) Z.physik.Chem., 33, 453-476.
Ageno, F. and Valla, E.
(1911) Atti accad.Lincei, 20, II, 706.
(1912) ist.Ven.[VIII], 14, II, 331.
(1913) Gazz.chim.ital., 43, II, 168.
d'Agostino, E.
(1910) Rend. soc.chim.ital. (Roma), 2,
II, 171.
Aignan, A. and Dugas, E.
(1899) Compt.rend., 129, 643.
Alexejew, Wladimir. (Alexejeff.)
(i886)Wied.Ann.Physik.,28,305,338.
Allen, E. T. and White, W. P.
(1909) Am.Jour.Sci.[4], 27, I.
Altschul.
(1896) Monatsh.Chem., 17, 575.
Alluard.
(1864) Compt.rend., 59, 500.
(1865) Liebig's Ann., 133, 292.
Amadori, M.
(1912) Atti accad.Lincei, 21, II, 67,
184, 769, 690.
(i9i2a) Atti accad.Lincei, 21, I, 467,
667-73.
(1913) Atti accad.Lincei, 22, I, 453,
609; 22, II, 333.
(1915) Atti accad.Lincei, 24, II, 204.
Amadori, M. and Becarelli, R.
(1912) Atti accad.Lincei, 21, II, 698.
Amadori, M. and Pampanini, G.
(1911) Atti accad.Lincei, 20, II, 475,
572.
Amat, L.
(1887) Compt.rend., 105, 809.
Anderson.
(1888-89) Proc.Roy.Soc.(Edin.), 16,
319.
Andrae.
(1884) J.prakt.Chem. [2], 29, 456.
Andrews, L. W. and Ende, C.
(1895) Z.physik.Chem., 17, 136.
Anon.
(1903) Bull.soc.pharm. (Bordeaux),
p. 7.
(1904) Pharm.Jour.(Lond.), 72, 77.
1 The abbreviations of the names of the journals referred to in this index agree,
for the most part, with those adopted for Chemical Abstracts. They will, there-
fore, be readily understood in all but a few cases. One abbreviation which differs
from that used in Chemical Abstracts is Proc. k. Akad. Wet. (Amst.) instead of
Proc. Acad. Sci. Amsterdam. It refers to the English edition of Verslag koninkl
ke Akademie van Wetenschappen te Amsterdam.
Another abbreviation which has been adopted for the present index is the use
of "Tables arinuelles " for the French title, Tables annuelles de Constantes et
Donnees Numerique de Chemie, de Physique et de Technologic, of the Interna-
tional Tables of Constants and Numerical Data published in Paris under the
direction of the general secretary, Professor Marie. Of the three volumes which
have been published, Vol. I contains data for the year 1910 and was issued in
1912; Vol. 2 is for the year 1911 and appeared in 1913; and Vol. 3 contains data
for 1912 and was issued in 1914.
785
AUTHOR INDEX
Anthony, C. G.
(1916) Bonfort's Wine and Spirit
Circular, Apr. loth,
von Antropoff, A.
(1909-10) Proc.Roy.Soc. (London),
A 83, 474-83.
Armstrong, H. E. and Eyre, J. V.
(1910-11) Proc. Roy. Soc. (London),
(A), 84, 123-135.
(1913) Proc. Roy. Soc. (London), (A),
88, 234.
Armstrong, H. E., Eyre, J. V., Hussey,
A. V., and Paddison, W. P.
(1907) Proc. Roy. Soc. (London), (A),
79i 564-576.
Ange, see Auge.
d'Ans, see D'Ans.
d'Anselme.
(1903) Bull.soc.chim. [3], 29, 372.
Archibald, E. H., Wilcox, W. G. and
Buckley, B. G.
(1908) J.Am.Chem.Soc., 30, 747-60.
Arctowski, H.
(1894) Z.anorg.Chem., 6, 267, 404.
(1895) Compt.rend., 121, 123.
(1895-6) Z.anorg.Chem., n, 272-4.
Armit, H. W.
(1907) Jour.Hygiene, 7, 525-51.
Arndt, K.
(1907) Ber., 40, 427.
Arndt, K. and Loewenstein, W.
(1909) Z.Elektrochem., 15, 784-90.
Arrhenius, S.
(1893) Z.physik.Chem., n, 396.
Arth, G. and Cretien.
(1906) Bull.soc.chim. [3], 35, 778.
Artmann, P.
£1912-13) Z.anorg.Chem., 79, 333.
(1915) Z.anal.Chem., 54, 90.
Aschan, Ossian.
(1913) Chem.Ztg., 37, 1117.
AssBlin, E.
(1873) Compt.rend., 76, 884.
(1873) Jahresber.Chem., 1063.
Aten, A. H. W.
(1905) Z.anorg.Chem., 47, 387.
(1905-06) Z.physik.Chem., 54, 86,
124.
(1909) Z.physik.Chem., 68, 41.
(1912) Proc.k.Akad.Wet. (Amst.), 15,
(1912-13) Z.physik.Chem., 81, 268.
(1913) Z.physik.Chem., 83, 443.
(1914) Z.physik.Chem., 86, 1-35.
(i9Ha) Z.physik.Chem., 88, 321-379.
Atkins, W. R. G. and Werner, E. A.
(1912) J.Chem.Soc.(Lond.), 101,1167.
Aubert, A. B.
(1902) J.Am.Chem.Soc., 24, 690.
Auerbach, F. §
(1903) Z.anorg.Chem., 37, 353-77.
(1904) Z.Elektrochem., 10, 163.
Auerbach, F. and Barschall, H.
(1908) Arb.Kais.Gesundheitsamt.,
27, 183-230.
(1908) Chem.Abs., 2, 1125.
Auge, E.
(1890) Compt.rend., no, 1139.
Bagster, L. S.
(1911) J.Chem.Soc.(Lond.), 99, 1218.
Bahr, F.
(1911) Z.anorg.Chem., 71, 85.
Bakunin, M. and Angrisani, T.
(1915) Gazz.chim.ital., 45, I, 204.
Ballo, Rezso.
(1910) Z.physik.Chem., 72, 439.
Baly.
(1900) Phil.Mag. [5], 49, 517.
Bancroft, W. D.
(1895) Phys. Rev., 3, 31, 122, 193,
205.
Banthisch.
(1884) J.prakt.Chem., [2], 29, 54.
Barker, T. V.
(1908) J.Chem.Soc.(Lond.), 93, 15.
Barnes, H. T.
(1900) J.Phys.Chem., 4, 19.
Barnes, H. T. and Scott.
(1898) J.Phys.Chem., 2, 542.
Baroni, T. and Barlinetto, V.
(1911) Giorn.farm.chim., 60, 193.
(1911) " Tables annuelles," 2, 474.
Barre, M.
(1909) Compt.rend., 148, 1604-6;
149, 292.
(1910) Compt.rend., 150, 1321, 1599;
151, 871-3.
(1911) Ann.chim.phys., [8], 24, 149-
167, 202, 210-223.
(1912) Bull.soc.chim. [4], n, 646.
Basch.
(1901) Dissertation (Berlin), p. 17.
Baskov, A.
(1913) Jour.Russ.Phys.Chem.Soc.,
45, 1608.
(1914) Ann.inst.Electrotechnique
(Petrograd), n, 143.
(1915) J.Russ.Phys.Chem.Soc., 47,
1533-5-
Bassett, H. Jr.
(1908) Z.anorg.Chem., 59, 1-55.
(1917) J.Chem.Soc.(Lond.), in,
620-42.
Bassett, H. Jr. and Taylor, H. S.
(1912) J.Chem.Soc.(Lond.), 101, 576.
(1914) J.Chem.Soc.(Lond.), 105,
1926-41.
Bathrick.
(1896) J.Phys.Chem., I, 159.
Battelli and Martinetti.
(1885) Atti accad.sci.Torino, 20,
844.
Baubigny, H.
(1908) Bull.soc.chim. [4], 3, 772.
(1908) Compt.rend., 146, 1263.
786
AUTHOR INDEX
Baud, E.
(1909) Bull.soc.chim. [4], 5, 1022.
(1909) Compt.rend., 148, 96.
(1912) Ann.chim.phys. [8], 27, 95-8.
(i9i2a) Bull.soc.chim. [4], n, 948.
(i9i3a) Compt.rend., 156, 317.
(i9i3b) Ann.chim.phys. [8], 29, 131-
136.
(19130) Bull.soc.chim. [4], 13, 436.
(1913) Ann.chim.phys., [8], 29, 131.
Baud, E. and Gay, L.
(1910) Compt.rend., 150, 1688.
(1911) Bull.soc.chim. [4], 9, 119.
Baum, Fritz.
(1899) Archiv. exp.Path.u Pharm.,
42, 119-137-
Baume, G.
(1911) J.chim.phys., 9, 245.
(1914) J.chim.phys., 12, 216.
Baume, G. and Borowski, W.
(1914) J.chim.phys., 12, 276-81.
Baume, G. and Georgitses, N.
(1912) Compt.rend., 154, 650.
(1914) J.chim.phys., 12, 250.
Baume, G. and Germann, F. O.
(1911) Compt.rend., 153, 569.
(1914) J.chim.phys., 12, 242.
Baume, G. and Pamfil, G. P.
(1911) Compt.rend., ?52> IO95-
(1914). J.chim.phys., 12, 256.
Baume, G. and Perrot, F. L.
(1911) Compt.rend., 152, 1763-5.
(1914) J.chim.phys., 12, 225.
Baume, G. and Tykociner, A.
(1914) J.chim.phys., 12, 270-5.
Baup.
(1858) Ann.chim.phys. [3], 53, 468.
Baxter, G. P., Boylston, A. C. and Hub-
bard, R. A.
(1906) J.Am.Chem.Soc., 28, 1343. .
Bechold and Ziegler.
(1910) Z.angew.Chem., 23, 29.
Beck, K.
(1904) Z.physik.Chem., 48, 657.
Beck, K. and Stegmiiller, Ph.
(1910) Arb.Kais.Gesundheitsamt.,
34, 447-
(1911) Z.Elektrochem., 17, 843-48.
Beckmann, E. and Stock, A.
(1895) Z.physik.Chem., 17, 130.
Behrend, R.
(1892) Z.physik.Chem., 10, 265.
(1893) Z.physik.Chem., u, 466.
Bell.
(1867) Chem.News., 16, 69.
Bell, J. M.
(1905) J. Phys. Chem., 9, 544.
(1911) J.Am.Chem.Soc., 33, 940.
Bell, J. M. and Buckley, M. L.
(1912) J.Am.Chem.Soc., 34, 10.
Bell, J. M. and Taber, W. C.
(1907) J.Phys.Chem., n, 637-8.
(1908) J.Phys.Chem., 12, 174.
Bellucci, I.
(1912) Atti accad.Lincei, [5], 21, II,
610.
(1913) Gazz.chim.ital., 43, I, 521.
Bellucci, I. and Grassi, L.
(1913) Gazz.chim.ital., 43, II, 712.
(1913) Atti accad.Lincei [5], 22, II,
676.
(1914) Gazz.chim.ital., 44, I, 559.
Benedicks.
(1900) Z.anorg.Chem., 22, 409.
Bennett, R. R.
(1912) Pharm. Jour. (Lond.), 89, 146.
Bergius, F.
(1910) Z.physik.Chem., 72, 338-61.
Berju and Kosminiko.
(1904) Landw.Vers.Sta., 60, 422.
Berkeley, Earl of.
(1904) Phil.Trans.Roy.Soc.(Lond.),
203, A., 189-215.
Berkeley, Earl of, and Appleby, M. P.
(1911) Proc.Roy.Soc., 85, 503.
Bernardis, G. B.
(1912) Atti accad.Lincei [5], 21, II,
442.
Bernfeld.
(1898) Z.physik.Chem., 25, 72.
Bertheaume, J.
(1910) Compt.rend., 150, 1064.
Berthelot, M.
(1904) Ann.chim.phys. [8], 3, 146.
(1904) Compt.rend., 138, 1649.
Berthelot, M. and Jungfleisch.
(1872) Ann.chim.phys. [4], 26, 400.
Bertrand.
(1868) Monit.Scient. [3], 10, 477.
Beurath, A.
(1912-3) J.prakt.Chem. [2], 87, 423.
Bevade, J. (Bewad).
(1884) Ber., 17, R., 406.
(1885) Bull.soc.chim. [2], 43, 123.
Bianchini, G.
(1914) Atti accad.Lincei [5], 23, I,
609.
Biginelli, P.
(1908) Gazz.chim.ital., 38, I, 559-82.
Billitzer, J.
(1902) Z.physik.Chem., 40, 535.
Biltz, W.
(1903) Z.physik.Chem., 43, 42.
Biltz, W. and Marcus, E.
(1911) Z.anorg.Chem., 71, 167.
Biltz, W. and Wilke.
(1906) Z.anorg.Chem., 48, 299.
Birger, Carlson, see Carlson, Birger.
Biron.
(1899) J.Russ.Phys.Chem.Soc., 31,
5T7-
Bissell, D. W. and James, C.
(1916) J.Am.Chem.Soc., 38, 873.
Blanksma, J. J.
(1910) Chem.Weekblad., 7, 418.
(1912) Chem.Weekblad., 9,
787
AUTHOR INDEX
Blanksma, J. J.
(1913) Chem.Weekblad., 10, 136.
(1914) Chem.Weekblad., n, 28.
Blarez.
(1891) Compt.rend., 112, 434, 939,
1213.
Blarez and Deniges.
(1887) Compt.rend., 104, 1847.
Bodlander, G.
(1891) Z.physik.Chem., 7, 317, 361.
(1892) Z.physik.Chem., 9, 734.
(1898) Z.physik.Chem., 27, 66.
Bodlander, G. and Eberlein, W.
(1903) Ber., 36, 3948.
Bodlander, G. and Fittig, R.
(1901-02) Z.physik.Chem., 39, 597-
612.
Bodlander, G. and Storbeck.
(1902) Z.anorg.Chem., 31, 22, 460.
Bodtker, E.
(1897) Z.physik.Chem., 22, 510, 570.
Boeke, H. E.
(1907) Z.anorg.Chem., 50, 335.
(1911) NJahr.Min., i, 48, 61.
(1911) Sitzber.k.Akad.Wiss. (Berlin),
24, 632-8.
Boeseken, J.
(1912) Rec.trav.chim., 31, 354-360.
Boeseken, J. and Carriere.
(1915) Rec.trav.chim., 34, 181.
Boeseken, J. and Waterman, H.
(1911) Verslag.k.Akad.Wet.(Am3t.),
2<>» SSS-
(1912) Proc.k.Akad.Wet.(Amst.), 14,
620.
Boericke, F.
(1905) Z.Elektrochem., n, 57.
Bogdan, P.
(1902-3) Ann. Sci. Univ. Jassy, 2, 47.
(1905) Z.Elektrochem., n, 825.
(1906) Z.Elektrochem., 12, 490.
Bogitch, B.
(1915) Compt.rend., 161, 790-1.
Bogojawlensky, A. and Winogradow,N.
(1907) Z.physik.Chem., 60, 433.
(1916) Sitzber.Natur.Ges. Univ. Dor-
pat., 15, 230-37.
Bogojawlensky, A., Winogradow, N.
and Bogolubow.
(1906) Sitzber.Natur.Ges. (Dorpat.),
(1916) Sitzber.Natur.Ges. (Dorpat.),
15, 216-29.
Bogorodsky.
(1894) J.Russ.Phys.Chem.Soc., 26,
209.
(1894) Chem.Centralbl., II, 514.
Bogousky.
(1905) J.Russ.Phys.Chem.Soc., 37,
92.
Bohling.
(1884) Z.anal.Chem., 23, 518.
Bohr, C.
(1899) Wied.Ann.Physik. [3], 68,
50.3-
(1910) Z.physik.Chem., 71, 47-50.
Bohr, C. and Bock.
(1891) Wied.Ann.Physik [2], 44,
318.
Boks.
(1902) Dissertation, Amsterdam.
Bonner, W. D.
(1910) J.Phys.Chem., 14, 738-789.
Bonsdorff, W.
(1904) Z.anorg.Chem., 41, 180.
Bornwater, J. T. and Holleman, A. F.
(1912) Rec.trav.chim., 31, 230.
Borodowski, W. and Bogojawlenski.
(1904) J.Russ.Phys.Chem.Soc., 36,
559-6o.
Botta.
(1911) Zentralbl.Min.Geol., p. 123.
Bottger, W.
(1903) Z.physik.Chem., 46, 521-619.
(1906) Z.physik.Chem., 56, 83-94.
Boubnoff, N. and Guye, Ph. A.
(1911) J.chim.phys., 9, 304.
Bougault.
(1903) J.pharm.chim. [6], 18, 116.
Boulouch, R.
(1902) Compt.rend., 135, 165.
(1906) Compt.rend., 142, 1045.
Bourgoin.
(1874) Bull.soc.chim. [2], 21, no.
(1878) Ann.chim.phys. [5], 13, 406;
I5> 165.
(1884) Bull.soc.chim. [2], 42, 620.
Boutaric, A.
(1911) Compt.rend., 153, 876-7.
Bowen, N. L.
(1914) Am.Jour.Sci. [4], 38, 207-264.
Bowen, N. L. and Anderson, Olaf .
(1914) Am.Jour.Sci. [4], 37, 487.
Boyle, Mary.
(1909) J.Chem.Soc.(Lond.), 95, 1696.
Boyle, R. W.
(1911) Phil. Mag. [6], 22, 840-854.
Bradley, W. P. and Alexander, W. B.
(1912) J.Am.Chem.Soc., 34, 17.
Bramley, A.
(1916) J.Chem.Soc.(Lond.), 109,
469-96.
Brand, H.
(1911) Neues Jahrb.Min.Geol.(Beil.
Bd.), 32, 627-700.
(1912) Zentralbl.Min.Geol.and Pal.,
26-32.
(1913) Neues Jahrb.Min.Geol., I,
9-27.
Brandan.
(1869) Liebig's Ann., 151, 340.
Braun, L.
(1900) Z.physik.Chem., 33, 732.
Brauner, B.
(1898) J.Chem.Soc.(Lond.), 73, 955.
788
AUTHOR INDEX
Bray, Wm. C.
(1905-06) Z.physik.Chem., 54, 569-
608.
Bray, W. C. and Connolly, E. L.
1(1910) J.Am.Chem.Soc., 32, 937.
(1911) J.Am.Chem.Soc., 33, 1485.
Bray, W. C. and MacKay, G. M. T.
(1910) J.Am.Chem.Soc., 32, 914,
1207.
Bray, Wm. C. and Winninghoff.
(1911) J.Am.Chem.Soc., 33, 1663.
Breithaupt, J.
( ) These, Univ. of Geneve., 38,
No. 446.
Briegleb.
(1856) Liebig's Ann., 97, 95.
Brinton, Paul H. M. P.
(1916) J.Am.Chem.Soc., 38, 2365.
Brissemoret, M.
(1898) J.pharm.chim. [6], 7, 176-8.
Bronsted, J. N.
(1906) Z.physik.Chem., 55, 377.
(1909) 7th Int. Congress Applied
Chem., 10, no.
(1911) Z.physik.Chem., 77, 132.
(1912) Z.physik.Chem., 80, 208, 214.
Brown, J. C.
(1907) Proc.Chem.Soc., 23, 233.
(1907) J.Chem. Soc.(Lond-), 91,
1826-31.
Brown, O. W.
(1898) J.Phys.Chem., 2, 51.
Browning and Hutchins.
(1900) Z.anorg.Chem., 22, 380.
Bruner, L.
(1898) Z.physik.Chem., 26, 147.
Bruner, L. and Zawadski, J., el al.
(1909) Bull.Internat.acad.Sci. Cra-
covie, [3], 9, A, 267-312, 377.
(1910) Z.anorg.Chem., 67, 454-5.
(1910) Chem. Abs., 4, 980, 2758.
Bruni, G.
(1898) Gazz.chim.ital., 28, II, 508-
529-
(1899) Atti accad.Lincei, [5], 8, II,
141.
(1900) Gazz.chim.ital., 30, I, 25-35.
Bruni, G. and Berti, P.
(1900) Gazz.chim.ital., 30, II, 324.
Bruni, G. and Finzi, F.
(1905) Gazz.chim.ital., 35, II, in-
131-
Bruni, G. and Gorni, F.
(1899) Atti accad.Lincei, [5], 8, II, 188.
(1900) Atti accad.Lincei, [5], 9, 11,326.
Bruni, G. and Meneghini.
(1909) Z.anorg.Chem., 64, 193.
(1910) Gazz.chim.ital., 40, I, 682.
de Bruyn, C. A. Lobry.
(1890) Rec.trav.chim., 9, 188.
(1892) Z.physik.Chem., 10, 782-789.
(1892) Rec.trav.chim., n, 29, 112-
156.
de Bruyn, C. A. Lobry.
(1894) Rec.trav.chim., 13, 116, 150.
(1899) Rec.trav.chim., 18, 87.
(1900) Z.physik.Chem., 32, 63, 85,
92, 101.
(1903) Rec.trav.chim., 22, 411.
de Bruyn, C. A. Lobry, and van Eken-
stein, W. A.
(1899) Rec.trav.chim., 18, 150.
(1900) Rec.trav.chim., 19, 7.
Bubanovic, F.
(1913) Med.K.Vetenskapsakad.No-
belinst, 2, No. 33.
'(1913) Chem.Abs., 7, 2886.
Bube, Kurt.
(1910) Z.anal.Chem., 45, 525-96.
Buchner, E. H.
(1865) Sitzber.k.Akad.Wiss.(Wein),
52, 2, 644.
(1905-06) Z.physik.Chem., 54, 665-
88.
Buchner, E. H. and Karsten, B. J.
(1908-9) Proc.k.Akad.Wet.(Amst.),
n, 504.
Buchner, E. H. and Prins, Ada.
(1912-13) Z.phys.Chem., 81, 113-120
Bugarszky, S.
(1910) Z.physik.Chem., 71, 753.
Bunsen, Robert.
(1877) " Gasometrische Methoden,"
2nd Ed.
Bunsen-Heurich.
(1892) Z.physik.Chem., 9, 438.
Bylert, V.
( ) These, Amsterdam.
Cabot, G. L.
(1897) J.Soc.Chem.Ind., 16, 417.
Cady, H. P.
(1898) J.Phys.Chem., 2, 168, 206.
Caille.
(1909) Compt.rend., 148, 1461.
Calcagni, G.
(1912) Gazz.chim.ital., 42, II, 653,
661.
(i9i2a) Atti accad.Lincei, [5], 21, II,
72.
Calcagni, G. and Mancini, G.
(1910) Atti accad.Lincei, [5], 19, II,
424.
Calcagni, G. and Marotta, D.
(1912) Gazz.chim.ital., 42, II, 669-
680.
(1912) Atti accad.Lincei, [5], 21, II,
93, 243, 284.
(1913) Gazz.chim.ital., 43, II, 380.
(1913) Atti accad.Lincei, [5], 22, II,
373, 443-
(1914) Gazz.chim.ital., 44, I, 487.
Callender and Barnes.
(1897) Proc.Roy.Soc., 62, 149.
Calvert, H. T.
(1901) Z.physik.Chem., 38, 521-540.
789
AUTHOR INDEX
Calzolari, F.
(1912) Gazz.chim.ital., 42, II, 85-92.
( ) Acc.sc.med.e.nat.di Ferora,
85, 150.
Cambi, L.
(1912) Atti accad.Lincei, [5], 21, I,
776, 791.
(1912) Atti accad.Lincei, [5], 21, II,
839-
Cambi, L. and Speroni, G.
(1915) Atti accad.Lincei, [5], 24, I,
736.
Cameron, F. K.
(1898) J.Phys.Chem., 2, 413.
(1901) J.Phys.Chem., 5, 556.
Cameron, F. K. and Bell, J. M.
(1905) J.Am.Chem.Soc., 27, 1512.
(1906) J.Am.Chem.Soc., 28, 1220,
1222.
(i9o6a) J.Phys.Chem., 10, 210.
(1907) J.Phys.Chem., n, 363.
(1910) J.Am.Chem.Soc., 32, 869.
Cameron, F. K., Bell, J. M., and Robin-
son, W. O.
(1907) J.Phys.Chem., n, 396-420.
Cameron, F. K. and Breazeale, J. F.
(1903) J.Phys.Chem., 7, 574.
(1904) J.Phys.Chem., 8, 335.
Cameron, F. K. and Patten, H. E.
(1911) J.Phys.Chem., 15, 67.
Cameron, F. K. and Robinson, W. O.
(1907) J.Phys.Chem., n, 577, 641,
691.
(i9O7a) J.Phys.Chem., n, 273-8.
(1909) J.Phys.Chem., 13, 157, 251.
Cameron, F. K. and Seidell, A.
(1901) Bull. No. 18, Division of Soils,
U. S. Dept. Agr.
(igoia) J.Phys.Chem., 5, 643.
(1902) J.Phys.Chem., 6, 50.
Campetti, A.
(1901) Atti accad.Lincei., [5], 10, II,
99-102.
(1902) Z.physik.Chem., 41, 109,
(abstract).
(1917) Atti accad.sci.Torino, 52,
114-21.
Campetti, A. and Del Grosso, C.
(1913) Nuovo cimento, [6], 6, 379-
417
(1913) Mem. R.accad.Sci. (Torino),
[II], 61, 187.
(1911) "Tables annuelles," 2, 433.
Cantoni, H. and Basadonna.
(1906) Bull.soc.chim., [3], 35, 731.
Cantoni, H. and Diotalevi, D.
(1905) Bull.soc.chim., [3], 33, 27-36.
Cantoni, H. and Goguelia, G.
(1905) Bull.soc.chim., [3], 33, 13.
Cantoni, H. and Jolkowsky.
(1907) Bull.soc.chim. [4], i, 1181.
Cantoni, H. and Passamanik.
(1905) Ann.chim.anal.appl., 10, 258.
Cantoni, H. and Zachoder.
(1905) Bull.soc.chim., [3], 33, 747.
Cap and Garot.
(1854) J.pharm.chim., [3], 26, 81.
Capin, J.
(1912) Pharm.Jour.(Lond.), 88, 65,
from (1911) Bull.soc.
pharm. (Bordeaux), 414.
Carlinfanti, E. and Levi-Malvano, M.
(1909) Gazz.chim.ital., 39, II, 353-
75-
Carlson, Birger.
(1910) Klason-Festschrift, 247-66
(Stockholm).
(1910) " Tables annuelles," i, 379.
Carnelly.
(1873) Liebig's Ann., 166, (116?),
155-
(1873) J.Chem.Soc.(Lond.), [2], n,
323-
Carnelly and Thomson.
(1888) J.Chem.Soc.(Lond.), 53, 799.
Caro.
(1874) Arch.Pharm., [3], 4, 145.
Carpenter.
(1886) J.Soc.Chem.Ind., 5, 286.
Carr, F. H. and Pyman, F. L.
(1914) J.Chem.Soc.(Lond.), 105,
1 602-1 1.
Carrara and Minozzi.
(1897) Gazz.chim.ital., 27, II, 955.
Carveth, H. R.
(1898) J.Phys.Chem., 2, 213.
Caspari, W. A.
(1915) J.Chem.Soc.(Lond.), 107,
162-171.
Cassuto, L.
(1913) Nuovo cimento, 6, 1903.
Cavazzi, A.
(1916) Gazz.chim.ital., 46, II, 122-35
(1917) Gazz.chim.ital., 47, II, 49-63.
Centnerszwer, M.
(1899) Z.physik.Chem., 29, 715.
(1910) Z.physik.Chem., 72, 437.
Centnerszwer, M. and Teletow, I.
(1903) Z.Elektrochem., 9, 799.
de Cesaris, P.
(1911) Atti accad.Lincei, [5], 20, I,
597, 749"
Chancel and Parmentier.
(1885) Compt.rend., 100, 473, 773-
Chandler, E. E.
(1908) J.Am.Chem.Soc., 30, 696.
Chattaway, F. D. and Lambert, Wm. J.
(1915) J.Chem.Soc.(Lond.), 107,
1768, 1776.
Chavanne, G. and Vos, J.
(1914) Compt.rend., 158, 1582.
Chikashigi, M.
(i9ii-i2)Mem.Coll.Sci.Eng.(Kyoto),
3, 197-206.
(1911) Z.anorg.Chem., 72, 109.
790
AUTHOR INDEX
Chikashigi, M. and Yamanchi, Y.
(1916) Mem.Coll.Sci. Kyoto, 1,341-7.
Chilesotti, A.
(1908) Atti accad.Lincei, [5], 17, II,
475-
Christensen.
(1885) J.prakt.Chem., [2], 31, 166.
Christoff, A.
(1905) Z.physik.Chem., 53, 321.
(1906) Z.physik.Chem., 55, 627.
(1912) Z.physik.Chem., 79, 459.
Christy, S. B.
(1901) Elektrochem.Ztschr., 7, 205.
Chugaev, L. and Khlopin, W.
(1914) Z.anorg.Chem., 86, 159.
Cingolani, M.
(1908) Gazz.chim.ital., 38, I, 305.
(1908) Atti accad.Lincei., [5], 17, I,
265.
Ciusa, R. and Bernard!, A.
(1910) Gazz.chim.ital., 40, II, 159.
Claasen, H.
(1911) Z.Ver.Zuckerind.,6i, 489-509.
Cleve.
(1866?) K. Svenska Vetenskaps-
Akad.Handl.(Stockholm),
10, 9, 7.
(1874) Bull.soc.chim., [2], 21, 344.
(1885) Bull.soc.chim., [2], 43, 166.
Cleve, Astrid.
(1902) Z.anorg.Chem., 32, 157.
Cloez.
(1903) Bull.soc.chim. [3], 29, 167.
Clowes, F. and Biggs, J. W. H.
(1904) J.Soc.Chem.Ind., 23, 358.
Cocheret, D. H.
(1911) Dissertation, Leiden.
(1911) "Tables Annuelles"2, 439,
444.
Cohen, Ernst.
(1900) Z.physik.Chem., 34, 189, 622.
(1903) Z.Elektrochem., 9, 433.
(1909) Z.Elektrochem., 15, 600.
Cohen, E. and Inouye, K.
(1910) Z.physik.Chem., 72, 411-424.
(1910) Chem.Weekblad., 7, 277.
Cohen, E., Inouye, K. and Euwen, C.
(1910) Z.physik.Chem., 75, 257.
Cohen, E. and Sinnige, L. R.
(1910) Trans. FaradaySoc., 5, 269.
Conn, E.
(1895) Z.physik.Chem., 18, 61.
Colani, A.
(1913) Compt.rend., 156, 1075, 1908.
(1916) Bull.soc.chim., [4], 19, 405.
(19163) Compt.rend., 163, 123-5.
(1917) Compt.rend., 165, 111-3,
234-6.
Colson, A.
(1907) Compt.rend., 145, 1167,.
Comanducci, E.
(1912) Rend.soc.chim.ital., [2], 4,
313.
de Coninck, Oechsner.
(1893) Compt.rend., 116, 758.
(1894) Compt.rend., 118, 471.
(1900) Compt.rend., 130, 1304; 131,
1219.
(1901) Bull.acad.roy.(Belgique), 350.
(1903) Ann.chim.phys., [7], 28, 7.
(1905) Chem.Centralbl., 76, II, 883.
(1905) Bull.acad.roy.(Belgique), pp.
257, 359-
(1906) Compt.rend., 142, 571.
Conroy.
(1898) J.Soc.Chem.Ind., 17, 104.
Cooper, H. C., Shaw, R. I., and Loomis,
N. E.
(1909) Am.Chem.Jour., 42, 461.
(1909) Ber., 42, 3991.
Copisarow, M.
(1915) Chem.News., 112, 247.
Coppadoro, A.
(1909) Gazz.chim.ital., 39, II, 625.
(1911) Rend.soc.chim.ital., [2], 30,
207.
(1912) Gazz.chim.ital., 42, I, 240.
(1912) Atti accad.Lincei, [5], 21, II,
842.
(1913) Gazz.chim.ital., 43, I, 138.
de Coppet, L. C.
(1872) Ann.chim.phys., [4], 25, 528,
532.
(1883) Ann.chim.phys., [5], 30, 417.
(1899) Ann.chim.phys., [7], 16, 275.
Corliss, Harry P.
(1914) J.Phys.Chem., 18, 681.
Cossa, A.
(1868) Ber., i, 138.
(1869) Z.anal.Chem., 8, 145.
Costachescu, N.
(1910) Ann.Sci.Univ.(Jassy), 7, I.
Coste, J. H.
(1917) J.Soc.Chem.Ind., 36, 846-53.
(1918) J.Soc.Chem.Ind., 37, 170.
Cottrell, et al
(1901) Sitzber.k.Akad.Wiss. (Berlin),
P- 1035.
Couch, J. F.
(1917) Am.Jour.Pharm., 89, 243-51.
Courtonne, H.
(1877) Ann.chim.phys., [5], 12, 569.
(1882) Compt.rend., 95, 922.
Cowper, R.
(1882) J.Chem.Soc.(Lond.), 41, 254.
Creighton, H. J. M., and Ward, W. H.
(1915) J.Am.Chem.Soc., 37, 2333.
Croft.
(1842) Phil.Mag., [3], 21, 356.
Crompton, H. and Walker, M.
(1912) J.Chem.Soc.(Lond.), 101, 958.
Crompton, H. and Whiteley, M. A.
(1895) J.Chem.Soc.(Lond.), 67, 327.
Crookes, Wm.
(1864) J.Chem.Soc.(Lond.), 2, 134.
791
AUTHOR INDEX
Crowell, R. D.
(1918) J.Am.Chem.Soc., 40, 455.
Cuno, E.
(1908) Ann.physik., [4], 25, 346-76.
(1908-09) Ann.physik., [4], 28, 663-4.
(1907) Ber.physik.Ges., 5, 735~8.
Curtis, H. A. and Titus, E. Y.
(1915) J.Phys.Chem., 19, 740.
Curtius and Jay.
(1889) J.prakt.Chem., [2], 39, 39.
Dahms, A.
(1895) Wied.Ann.Physik., 54,486-519.
(1896) Wied.Ann.der Physik., 60, 122.
(1899) Ann.chim.phys., [7], 18, 140.
Dakin, H. D., Janney, N. W. and
Wakemann, A. J.
(1913) J.Biol.Chem., 14, 241.
van Damm, W. and Donk, A. D.
(1911) Chem.Weekblad, 8, 848.
Dancer.
(1862) J.Chem.Soc.(Lond.), 15, 477.
D'Ans, J.
(1908) Ber., 41, 1776-7.
(1909) Z.anorg.Chem., 62, 129-167.
oga) Z.anorg.Chem., 63, 225-9.
ogb) Z.anorg.Chem., 65, 228.
19090) Z.anorg.Chem., 61, 91-5.
(1913) Z.anorg.Chem., 80, 235.
D'Ans, J. and Fritsche, O.
(1909) Z.anorg.Chem., 65, 231.
D'Ans, J. and Schreiner, O.
(1910) Z.anorg.Chem., 67, 437.
(i9ioa) Z.physik.Chem., 75, 95-107.
D'Ans, J., Shepherd, L. D'Arey and
Gunther, P.
(1906) Z.anorg.Chem., 49, 356-61.
D'Ans, J. and Siegler, R.
(1913) Z.physik.Chem., 82, 35-44.
Davidsohn, J. and Wrage, W.
(1915) Chem.Rev.Fett.Harz.Ind., 22,
9-14.
Davis, H. S.
(1916) J.Am.Chem.Soc., 38, 1169.
Dawson, H. M.
(1901) J.Chem.Soc.(Lond.), 79, 242.
(1902) J.Chem.Soc.(Lond.) 81, 1086-
1097.
(1904) J.Chem.Soc.(Lond.), 85, 467.
(1906) J.Chem.Soc.(Lond.), 89, 1668.
(1908) J.Chem.Soc.(Lond.), 93, 1310.
(1909) Z.physik.Chem., 69, 110-122.
(i909a) J.Chem.Soc.(Lond.), 95,
370-81.
(19095) J.Chem.Soc.(Lond.), 95,874.
Dawson, H. M. and Gawler, R.
(1902) J.Chem.Soc.(Lond.), 81, 524.
Dawson, H. M. and Goodson, E. E.
(1904) J.Chem.Soc.(Lond.), 85, 796.
Dawson, H. M. and Grant.
(1901) J.Chem.Soc.(Lond.), 81, 512.
Dawson, H. M. and McCrae, J.
(1900) J.Chem.Soc.(Lond.), 77,
1239-62.
Dawson, H. M. and McCrae, J.
(igoia) J.Chem.Soc.(Lond.), 79, 493.
(1901 b) J.Chem.Soc.(Lond.), 79,
1069.
Dehn, Wm. M.
(1917) J.Am.Chem.Soc., 39, 1400.
(i9i7a) J.Am.Chem.Soc., 39, 1378.
De Jong (see de Jong).
Delange, Leon.
(1908) Bull.soc.chim., [4], 3, 910-5.
Delepine.
(1892) J.pharm.chim., [5], 25, 496.
(1895) Bull.soc.chim., [3], 13, 353.
(1908) Bull.soc.chim., [4], 3, 904.
Demarcay.
(1883) Compt.rend., 96, 1860.
Demassieux, N.
(1913) Compt.rend., 156, 892.
(1914) Compt.rend., 158, 183, 702.
Denham, H. G.
(1917) J.Chem.Soc.(Lond.), in, 39.
Derick, C. G. and Kamm, O.
(1916) J.Am.Chem.Soc., 38, 415.
Dernby, K. G.
(i9i8)Medd.k.Vetenkapsakad.Nobel
inst., 3, No. 1 8.
Derrien.
(1900) Compt.rend., 130, 722.
Deszathy.
(1893) Monatsh.Chem., 14, 249.
De Visser, L. E. O.
(1898) Rec.trav.chim., 17, 182, 346.
Dewey, F. P.
(1910) J.Am.Chem.Soc., 32, 318.
Dhar, N. and Datta, K.
(1913) Z.Elektrochem., 19, 584.
Diacon.
(1866) Jahrsber.Chem., 61.
Dibbits.
^1874) Z.anal.Chem., 13, 139.
74) J.prakt.Chem., [2], 10, 417,
439-
Dieterich.
(1890) Pharm.Centrh., 31, 395.
Dietz.
(1898) Pharm.Ztg., 43, 290.
(1899) Z.anorg.Chem., 20, 260.
(1899) Ber., 32, 95.
(1900) Wiss.Abt.p.t.Reichanstalt, ;,
433-
Dimroth, O. and Mason, F. A.
(1913) Liebig'sAnn., 399, 108.
Ditte, A.
\io/$} v^umpt.i ciiu.
(1877) Compt.rend.
(1881) Compt.rend.
(1881) Ann.chim.ph
(1896) Compt.rend.
(1897) Compt.rend.
OU, 1 l<Jif.
85, 1069.
92, 242, 718.
ys., [5], 24, 226.
123, 1282.
124, 30.
T-_1 _
(1898) Ann.chim.phys., [7], 14, 294.
Dittmar.
(1888) J.Soc.Chem.Ind., 7, 730.
792
AUTHOR INDEX
Dittrich, C.
(1899) Z.physik.Chem., 29, 485.
Ditz, H. and Kanhauser, F.
(1916) Z.anorg.Chem., 98, 128-40.
Divers.
(1870) J.Chem.Soc.(Lond.), 23, 171.
(1899) J.Chem.Soc.(Lond.), 75, 86.
Doerinckel, F.
(1907) Metallurgie, 8, 201-9, 408.
Dolezalek, F. and Finckli, K.
(1906) Z.anorg.Chem., 51, 320-7.
Dolgolenko, W.
(1907) Jour.Russ.Phys.Chem.Soc. 39,
841.
Dolinski, J. H.
(1905) Ber., 38, 1835.
Donath, E.
(1911) Chem.Ztg., 35, 773~4-
Donk, A. D.
(1908) Chem.Weekblad, 5, 529, 629,
767.
(1916) Chem.Weekblad, 13, 92-97.
Donk, M. G.
(1905) Bull. No. 90, Bureau Chem.
U. S. Dept. Agr.
Donnan, F. G. and Burt, B. C.
(1903) J.Chem.Soc.(Lond.), 83,- 335.
Donnan, F. G. and Thomas, J. S.
(1911) J.Chem.Soc.(Lond.),99, 1788.
Donnan, F. G. and White, A. S.
(1911) J.Chem.Soc.(Lond.), 99, 1669.
van Dorp, G. C. A.
(1910) Z.physik.Chem., 73, 284-289.
(1911) Chem.Weekblad., 8, 269.
(1912) 8th Internat.Cong.Appl.
Chem., 22, 239.
(1913-14) Z.physik.Chem., 86, 109.
Dott, D. B.
(1906) Pharm..
(1907) Pharm.]
(1910) Pharm/
(1912) Pharm..
our.(Lond.), 76, 345.
our.(Lond-), 78, 79.
our.(Lond.), 85, 795.
our.(Lond.), 88, 424.
Doumer and Deraux.
(1895) J- pharm.chim., [6], i, 50.
Doyer, J. W.
(1890) Z.physik.Chem., 6, 481.
Draper.
(1887) Chem.News., 55, 169.
Dreyer, F.
(1913) Ann.Inst.Polyt.(Petrograd),
20, 326.
Dreyer, F. and Rotarski.
(1905-06) Z.physik.Chem., 54, 356.
Driot.
(1910) Compt.rend., 150, 1426.
Drucker, K.
(1901) Z.anorg.Chem., 28, 362.
(1912) Z.Elektrochem., 18, 246.
Drucker, K. and Moles, E.
(1910) Z.physik.Chem., 75, 405.
Duboin, A.
(1905) Compt.rend., 141, 385.
Duboin, A.
(1906) Compt.rend., 142, 395, 573,
887, 1338.
Dubois and Fade.
(1885) Bull.soc.chim., [2], 44.
Dubowitz, H.
(1911) Seifensieder Ztg., 38, 1164,
1208.
( ) Vegnesceti lapok., 6, 397.
Dubrisay, Rene.
(1911) Compt.rend., 153, 1077.
(1912) Compt.rend., 154, 431.
Dubroca, M.
(1904) J.chim.phys., 2, 447.
(1907) J.chim.phys., 5, 463-87.
Dukelski, M. P.
(1906) Z.anorg.Chem., 50, 42.
(1907) Z.anorg.Chem., 53, 327~337J
54, 45—9.
(1907) J.Russ.Phys.Chem.Soc., 39,
975-88.
(1909) Z.anorg.Chem., 62, 114-8.
Dunn.
(1882) Chem.News, 45, 272.
Dunningham, A. C.
(1912) J.Chem.Soc.(Lond.), 101,
J.Chem.Soc.(Lond.), 105,
368-79, 73*3, 2630.
Dunnington and Long.
(1899) Am.Chem.Jour., 22, 217.
Dunstan, W. R. and Umney, J. C.
(1892) J.Chem.Soc.(Lond.), 61, 391.
Dupre and Bialas.
(1903) Z.angew.Chem., 16, 55.
Dutilh, H.
(i9i2)Verh.k.Akad.Wet.(Amst.),[n]
4,60.
(1912) " Tables annuelles," 3, 336.
Ebelmen.
(1852) Liebig's.Ann., [3], 5, 189.
Eder.
(1876) Dingier polyt.J., 221, 89, 189.
(1878) J.prakt.Chem., [2], 17, 45.
(1880) Sitzber.k.Akad.Wiss.(Wien),
82, Abt. II, 1284.
Efremov, N. N.
(1912) Ann. Inst. Polytechnic (Petro-
grad), 18, 391.
(1913) J.Russ.Phys.Chem.Soc., 45,
348-62.
(1915) Bull.acad.sci.Petrograd, 1309-
36.
(1916) Bull.acad.sci.Petrograd, 21-46.
Eggink, B. G.
(1908) Z.physik.Chem., 64, 492.
Ehlert, H. and Hempel, W.
(1912) Z.Elektrochem., 18, 727.
van Ekenstein, W. A. and de Bruyn,
C. A. Lobry.
(1896) Rec.trav.chim., 15, 225.
Emerson, W. H.
(1907) J.Am.Chem.Soc., 29, 1750-6.
793
AUTHOR INDEX
Emich.
(1884) Monatsh.Chem., 3, 336.
Emmerling.
(1869) Liebig's Annaien, 150, 257.
von Ende, C. L.
(1901) Z.anorg.Chem., 26, 148.
Engel.
(1886) Compt.rend., 102, 114.
(1887) Compt.rend., 104, 507, 913.
(1888) Ann.chim.phys., [6], 13, 348-
385-
(1889) Ann.chim.phys., [6], 17, 347.
(1891) Bull.soc.chim., [3], 6, 17.
Enell.
(1899) Pharm.Centralh., 38, 181.
(1899) Z.anal.Chem., 38, 386.
Engfeldt, N. O.
(1913) Farmaceutisk Revy, No. 8.
(1913) Apoth.Ztg., 28, 182.
(1913) Pharm.Jour.(Lond.), 90, 769.
aglish, S. and Turner, W. E. S.
(1915) J.Chem.Soc.(Lond.), 107,
774-83.
Enklaar, J. E.
(1901) Rec.trav.chim., 20, 183.
Ennis, A. J.
(1914) J.Chem.Soc.(Lond.), 105,
,350-64.
Eppel.
(1899) Dissertation, Heidelberg.
Erdmann.
(1893) Ber., 26, 2439.
Erdmann and Bedford.
(1904) Ber., 37, 1184.
Etard.
(1877) Compt.rend., 84, 1090.
(1884) Compt.rend., 98, 1434.
(1894) Ann.chim.phys., [7], 2, 526-
570; 3, 275.
von Euler, H.
(1903) Ber., 36, 2879, 3400.
(1904) Z.physik.Chem., 49, 315.
(1916) Z.physik.Chem., 97, 291.
von Euler, H. and Lb'wenhamn, E.
(1916) Z.Elektrochem., 22, 199-254.
(1916) Chem.Abs., 10, 3021.
(1917) Chem.Abs., n, 915.
Euwes, P. C. J.
(1909) Rec.trav.chim., 28, 298.
Ewers, Erich.
(1910) Milchwirschaft.Zentr., 6 (3?),
155-
van Eyk, see Van Eyk.
Fahrion, W.
(1916) Chem.Umschau, 23, 34-5.
Falciola, P.
(1910) Gazz.chim.ital., 40, II, 218.
(1910) Seifens Ztg., 38, 506.
Farmer, R. C.
(1901) J.Chem.Soc.(Lond.), 79, 865.
(1903) J.Chem.Soc.(Lond.), 83, 1446.
Farmer, R. C. and Warth, F. J.
(1904) J.Chem,Soc,(Lond.), 85, 1713.
Fastert, C.
(1912) Kali, [6], 454.
(1912) Neue.Jahrb.Min.Geol. (Beil.
Bd.), 33, 286.
Faucon, A.
(1909) Compt.rend., 148, 1189.
(1910) Ann.chim.phys., [8], 19, 70-
152.
Fauzer.
(1888) Math.u.Natur.Wiss.Ber.(Un-
garn), 6, 1.54.
de Fazi, R.
(1916) Gazz.chim.ital., 46, I, 345.
Fedotieff, P. P.
(1904) Z.physik.Chem., 49, 168.
(1910-11) Z.anorg.Chem., 69, 26.
(1911-12) Z.anorg.Chem., 73, 178.
Fedotieff, P. P. and Iljinsky.
(1913) Z.anorg.Chem., 80, 119.
Fedotieff, P. P. and Koltunoff, J.
(1914) Z.anorg.Chem., 85, 251.
Feit, W. and Przibylla, K.
(1909) Z.Kali, 3, 393-8.
Fenton, H. J. H.
(1898) J.Chem.Soc.(Lond.), 73, 479.
Ferchland.
(1902) Z.anorg.Chem., 30, 133.
Field.
(1859) J.Chem.Soc.(Lond.), n, 6.
Filehne, Wm.
(1907) Beitrage Chem.Physiol u.
Pathol., 10, 304.
Findlay, Alex.
(1901) J.Chem.Soc.(Lond.), 85, 403.
Findlay, Alex.
(1902) J.Chem.Soc.(Lond.), 81, 1217.
(1904) J.Chem.Soc.(Lond.), 85, 403.
(1908) Chem.News, 96, 163.
(1908) Analyst, 33, 391.
Findlay, Alex, and Creighton, H. J. M.
(1910) J.Chem.Soc.(Lond.), 97, 536-
61.
(1911) Biochem.Jour., 5, 294.
Findlay, A. and Hickmans, E. M.
(1907) J.Chem.Soc.(Lond.), 91, 905.
(1909) J.Chem.Soc.(Lond.), 95, 1389.
Findlay, A. and Howell, O. R.
(i9i4)J.Chem.Soc.(Lond.), 105, 291-
98.
(1915) J.Chem.Soc.(Lond.), 107,
282-4.
Findlay, Alex, and King, G.
(1913) J.Chem.Soc.(Lond.),i03,ii7o.
(1914) J.Chem.Soc.(Lond.), 105, 1297.
Findlay, Alex., Morgan, I. and Morris,
I. P.
(1914) J.Chem.Soc.(Load.), 105,
779-82.
Findlay, Alex, and Shen, B.
(1911) J.Chem.Soc.(Lond.), 99, 1313.
(1912) J.Chem.Soc.(Lond.), 101,
1459-68.
794
AUTHOR INDEX
Findlay, Alex, and Williams, T.
(1913) J.Chem.Soc.(Lond.), 103, 636.
Fischer, Emil.
(1906) Ber., 39, 4144-5.
Fisher, V. M.
(1914) J.Russ.Phys.Chem.Soc., 46,
1250-70.
Fisher, V. M. and Miloszewski, F.
(1910) Kosmos (Lemberg), 35, 538-
42.
(1910) Chem.Zentr., II, 1048.
Flaschner, O.
(1908) Z.physik.Chem., 62, 493-8.
(1909) J.Chem.Soc.(Lond.), 95, 668-
85-
Flaschner, O. and MacEwan, B.
(1908) J.Chem.Soc.(Lond.), 93, 1000.
Flaschner, O. and Rankin, I. G.
(1909) Sitzber.k.Akad.Wiss.(Wien),
118, 116, 695-722.
(1910) Monatsh.Chem., 31, 23-50.
Flawitzki, F.
(1909) J.Russ.Phys.Chem.Soc., 41,
739-
Fluckiger.
(1887) Arch.Pharm., [3], 25, 542.
Fock.
(1897) Z.Kryst.Min., 28, 365, 397.
Fokin, S. J.
(1912) J.Russ.Phys.Chem.Soc., 44,
163.
Fonda, G.
(1910) Dissertation, Karlsruhe.
Fontein, F.
(1910) Z.physik.Chem., 73, 212-251.
Fonzes-Diacon.
(1895) J.pharm.chim., [6], I, 59.
Foote, H. W.
(1903) Am.Chem.Jour., 30, 341.
(1903) Z.physik.Chem., 46, 81.
(1904) Am.Chem.Jour., 32, 252.
(1907) Am.Chem.Jour., 37, 124.
(1910) J.Am.Chem.Soc., 32, 618-22.
(1912) J.Am.Chem.Soc., 34, 880.
(1915) J.Am.Chem.Soc., 37, 290,
1 200.
Foote, H. W. and Andrew, I. A.
(1905) Am.Chem.Jour., 34, 153, 165.
Foote, H. W. and Chalker, W. C.
(1908) Am.Chem.Jour., 39, 564, 567.
Foote, H. W. and Haigh, F. L.
(1911) J.Am.Chem.Soc., 33, 459.
Foote, H. W. and Levy.
(1907) Am.Chem.Jour., 37, 119.
Foote, H. W. and Saxon, Blair.
(1914) J.Am.Chem.Soc., 36, 1695.
Foote, H. W. and Walden, P. T.
(1911) J.Am.Chem.Soc., 33, 1032.
Forbes, G. S.
(1911) J.Am.Chem.Soc., 33, 1937.
de Forcrand, R.
(1909) Compt.rend., 149, 719.
(i909a) Compt.rend., 149, 1344.
de Forcrand, R.
(1911) Compt.rend., 152, 1210,
(1912) Compt.rend., 154, 133.
(1912) Compt.rend., 155, 118, 1767.
de Forcrand, and Fonzes-Diacon.
(1902) Ann.chim.phys., [7], 26, 253.
Formanek.
(1887) Chem.Centralbl., 18, 270.
Forster.
(1892) Ber., 25.
Foster, B. and Neville, H. A. D.
(1910) Proc.Chem.Soc., 26, 236.
Fox, Chas. J. J.
(1902) Z.physik.Chem., 41, 458.
(1903) Z.anorg.Chem., 35, 130.
(1909) J.Chem.Soc.(Lond.), 95, 878-
89.
(i909a) Trans.Faraday Soc., 5, 68.
Fox, Chas. J. J. and Gauge, A. J. H.
(1910) J.Chem.Soc.(Lond.), 97, 377-
85-
Fraenckel, F.
(1907) Z.anorg.Chem., 55, 223-32.
Francois, M.
(1900) Compt.rend., 130, 1024.
Frankforter, G. B. and Cohen, Lillian.
(1914) J.Am.Chem.Soc., 36, 1103-34.
(1916) J.Am.Chem.Soc., 38, 1139.
Frankforter, G. B. and Frary, F. C.
(1913) J.Phys.Chem., 17, 402-473-
Frankforter, G. B. and Temple, S.
(1915) J.Am.Chem.Soc., 37, 2697-
2716.
Fraps, G. S.
(1901) Am.Chem.Jour., 27, 290.
Free, E. E.
(1908) J.Am.Chem.Soc., 30, 1366-74.
Fresenius.
(1846) Liebig's Annalen, 59, 118.
(1890) Z.anal.Chem., 29, 418.
(1891) Z.anal.Chem., 30, 672.
Freundlich, H. and Posnjak, E.
(1912) Z.physik.Chem., 79, 174.
Freundlich, H. and Richards, M. B.
(1912) Z.physik.Chem., 79, 692.
Freundlich, H. and Seal, A. N.
(1912) Z.Chem.Ind.Koll., u, 258.
Friedel.
(1869) Liebig's Ann., 149, 96.
Friedel and Gorgeu.
(1908) Compt.rend., 127, 590.
Friedel and Lachburg.
(1869) Bull. soc. chim., [2], 12, 92.
Friedlander, T.
(1901) Z.physik.Chem., 38, 389.
Friedrich, K.
(1907) Metallurgie, 4, 480, 671.
(1908) Metallurgie, 5, 114.
(1914) Metallurgie u.Erz., n, 196—
200.
Fronmuller.
(1878) Ber., n, 92.
795
AUTHOR INDEX
Fujimura, T.
(1914) Mem.Col.Sci.Kyoto, i, 63-68.
Fulda, W.
(1909) Arb.Kais.Gesundheitsamt, 30,
81.
Funk, R.
(1899) Z.anorg.Chem., 20, 412.
(1900) Wiss.Abh.p.t.Reichanstalt, 3,
440.
(igooa) Ber., 33, 3697.
Furcht, M. and Lieben, A.
(1909) Sitzber.k.akad.Wiss (Wien),
118, 116, 383.
(1909) Monatsh.Chem., 30, 555.
Fiirth.
(1888) Monatsh.Chem., 9, 311.
Galeotti, G.
(1906) Z.physiol.Chem., 48, 473.
Galeotti, C. and Giampalmo, G.
(1908) Z.Chem.Ind.Kolloide, 3, 118-
GarelU, F.
(1894) Gazz.chim.ital., 24, II, 263.
Garelli, F. and Calzolari, F.
(1899) Gazz.chim.ital., 29, 264.
Garside.
(1875) Chem.News, 31, 245.
Gaudechon, H.
(1910) Compt.rend., 150, 467.
Gaus.
(1900) Z.anorg.Chem., 25, 236.
Gay-Lussac.
(1819) Ann.chim.phys., n, 314.
Gazarolli and Thurnbalk.
(1881) Liebig's Ann., 209, 184.
Geffcken, G.
(1904) Z.physik.Chem., 49, 271, 296.
Geiger.
(1904) Dissertation (Berlin).
Gemsky, N.
(1914) Neues Jahrb.Min.Geol.(Beil.
Bd.), 36, 513-58.
von Georgievics, G.
(1913) Z.physik.Chem., 84, 358.
(1913) Monatsh.Chem., 34, 734.
(1915) Z.physik.Chem., 90, 54.
(1915) Monatsh.Chem., 36, 400.
Gerard.
(1901) /\nn.chim.anal., 6, 59.
Gerardin.
(1865) Ann.chim.phys., [4], 5, 129,
134, 147, 158.
Gerlach.
(1869) Z.anal.Chem., 8, 250, 281.
(1889) Z.anal.Chem., 28, 473.
Gibbs, H. D.
(1908) Philippine J.Sci., 3, A 357.
Gill, H. W.
(1914) J.Chem.Met.Soc.(S. Africa),
14, 290-2.
van Ginneken, P. J. H.
(1911) Verslag.k.Akad.Wet.(Amst.),
20, 337.
van Ginneken, P. J. H.
Z.Ver.Zuckerind, 62. 421-39.
Ginsberg, A. S.
(i9o6)Ann.Inst.Polyt.(Petrograd),6,
493-
(1908) Z.anorg.Chem., 59, 346.
(1909) Z.anorg.Chem., 61, 122.
Giolitti, F. and Bucci, G.
(1905) Gazz.chim.ital., 35, II, 162-9.
Giolitti, F. and Vecchiarelli, V.
(1905) Gazz.chim.ital., 35, II, 170.
Giran, H.
(1903) Jour.physique, [4], 2, 807.
(i9O3a) Ann.chim.phys., [7], 30, 249.
(1906) Compt.rend., 142, 398.
(1908) Compt.rend., 146, 270, 1270.
(1913) Bull.soc.chim., [4], 13, 1050.
Giraud, H.
(1885) Bull.soc.chim., [2], 43, 552.
von Girsewald, C. and Wdokitin, A.
(1909) Ber., 42, 856-9.
Giua, M.
(1914) Ber., 47, 1718-23.
(1915) Gazz.chim.ital., 45, I, 339,
557; II, 32, 348.
(1916) Gazz.chim.ital., 46, I, 289; II,
274.
(1916) Atti accad.Lincei, [5], 25, I,
99-105.
Gladstone.
(1854) J.Chem.Soc.(Lond.), 6, n.
Glauser, R. Th.
(1910) Z.anorg.Chem., 66, 437.
Glowezynski, Z.
(1914) Kolloidchem.Beihefte, 6, 147-
176.
Gniewosz, St. and Walfisz, Al.
(1887) Z.physik.Chem., i, 70.
Gockel.
(1897) Chem.Zentralbl., II, 401.
Godeffroy.
(1876) Ber., 9, 1337, 1369.
(1886) Z.oster.Apoth.Ver., No. 9.
Goldblum, H. and Stoffella, G.
(1910) J.chim.phys., 8, 154.
Goldblum, H. and Terlikowski, F.
(1912) Bull.soc.chim., [4], n, 146-
159-
Goldschmidt, H.
(1895) Z.physik.Chem., 17, 154.
(1898) Z.physik.Chem., 25, 95.
Goldschmidt, H. and Cooper, H. C.
(1898) Z.physik.Chem., 26, 715.
Goldschmidt, H. and Eckardt, M.
(1906) Z.physik.Chem., 56, 389.
Goldschmidt, H. and Sunde, E.
(1906) Z.physik.Chem., 56, 15.
Goodwin, W. L.
(1882) Ber., 15, 3039.
van der Goot, Tetta Polak.
(1913) Z.physik.Chem., 84, 419-450.
Gordon, V.
(1895) Z.physiLChem., 18, 1-16.
796
AUTHOR INDEX
Gore.
(1870) Proc.Roy.Soc., 18, 158.
Gori, G.
(1913) Boll. chim. farm., 52, 891-5.
(1915) Chem.Abs., 9, 1827.
Gortner, R. A.
(1914) Biochem.Bull., 3, 468-9.
Gothe, E.
(1915) Chem.Ztg., 39, 305-?-
Gott, B. S. and Muir, M. P.
(1888) J.Chem.Soc.(Lond.), 53, 138.
Grahmann, W.
(1913) Z.anorg.Chem., 81, 257-314.
Grant, A. J. and James, C.
'(1917) J.Am.Chem.Soc., 39, 934.
Green, W. F.
(1908) J.Phys.Chem., 12, 655-60.
Greenish, H. G.
(1900) Pharm.Jour.(Lond.)f 65, 190-
95-
Greenish, H. G. and Smith, F. A. U.
(1901) Pharm.Jour.(Lond.), 66, 774-
777, 806-811.
(1902) Pharm.Jour.(Lond.), 68, 510-
532.
(1903) Pharm.Jour.(Lond.), 71, 881.
Grehant, N.
(1894) Compt.rend., 118, 594.
Grb'ger, Max.
(1911) Z.anorg.Chem., 70, 135.
Groschuff, E.
(1901) Ber., 34, 3318.
(1903) Ber., 36, 1791, 4351.
(1908) Z.anorg.Chem., 58, 102, 113.
(1910) Chem.Weekblad., 7, 687.
(1911) Z.Elektrochem., 17, 348.
Grube, G.
(1914) Z.Elektrochem., 20, 342.
Gruttner, G.
(1914) Ber., 47, 3259.
Gudzeit, F.
(1908) Z.physiol.Chem., 56, 150-179.
(1909) Z.physiol.Chem., 60, 27, 38-
68.
Guerini, B.
(1912) Thesis, Lausanne.
Guerin, G.
(1913) J.pharm.chim., [7], 7, 438.
(1913) Pharm.Jour.(Lond.), 90, 769.
Guertler.
(1904) Z.anorg.Chem., 40, 337.
Guild, Ed. J.
(1907) Pharm.Jour.(Lond.), 78, 357.
Guntz, A. and Guntz, Jr., A. A.
(1914) Ann.chim., 2, 101.
Gurwitsch, L.
(1914) Z.physik.Chem., 87, 329.
Guthrie.
(1875) Phil.Mag.,
(1876) Phil.Mag.,
(1878) Phil.Mag.,
(1884) Phil.Mag.,
4], 49, 210.
i, 366.
5, 6, 40.
» "» ^
, 18,
30, 504.
Guthrie, A.
(1901) J.Soc.Chem.Ind., 20, 224.
Haber, F. and van Ordt, G.
(1904) Z.anorg.Chem., 38, 387.
Hager.
(1875) Chem.Zentralbl., 135.
(1903) " Handbuch de Pharmaceuti-
schen Praxis." 3rd. Ed.
Hahn.
(1877) Wyandotte Silver Smelting
Works.
Halban, Hans v.
(1913) Z.physik.Chem., 84, 129, 145.
Halberstadt.
(1884) Ber., 17, 2965.
Hamberg.
(1885) J. prakt.Chem., [2], 33, 433.
Hamberger, Anna.
(1906) Z.anorg.Chem., 50, 427.
Hamburger, E.
(1911) Arch.ges.Physiol.(Pfluger's),
143, 187.
von Hammel, A.
(1915) Z.physik.Chem., 90, 121.
Hampshire, C. H. and Pratt, W. R.
(1913) Pharm.Jour.(Lond.), 91, 140.
Hanausek.
(1887) J.pharm.chim., [5], 15, 509.
Hantzsch, A.
(1901) Verh.d.Vers.Deutsch Ntf.u.
Artze, 150-2.
(1902) Chem.Zentrbl., II, 922.
(1911) Ber., 44, 2006.
Hantzsch, A. and Sebalt, F.
(1899) Z.physik.Chem., 30, 258-99.
Hantzsch, A. and Vagt, A.
(1901) Z.physik.Chem., 38, 705-742.
Harkins, W. D.
(1911) J.Am.Chem.Soc., 33, 1807-
1827.
Harkins, W. D. and Clark, Geo. L.
(1915) J.Am.Chem.Soc., 37, 1816.
Harkins, W. D. and Paine, H. M.
(1916) J.Am.Chem.Soc., 38, 2709.
Harkins, W. D. and Pearce, W. T.
(1916) J.Am.Chem.Soc., 38, 2694,
2717.
Harkins, W. D. and Winninghoff, W. J.
(1911) J.Am.Chem.Soc., 33, 1827-36.
Harrass, Paul.
( 1 903) Arch .internat .Pharmacodyamie
et Therapie, n, 431-463.
Hartley, H.
(1908) J.Chem.Soc.(Lond.), 93, 741-5.
Hartley, H. and Barrett, W. H.
(1909) J.Chem.Soc.(Lond.), 95,
1178-85.
Hartley, H., Drugman, J., Vlieland, C.
A., and Bourdillon, Robt.
(I9I3) J.Chem.Soc.(Lond.), 103, 1749.
Hartley, H., Jones, B. M. and Hutchin-
son, G. A.
(1908) J,Chem.Soc.(Lond.), 93, 825.
797
AUTHOR INDEX
Hartley, H. and Thomas.
(1906) J.Chem.Soc.(Lond.), 89, 1028.
Haslam.
(1886) Chem.News., 53, 87.
Hasselblatt, M.
(1913) Z.physik.Chem., 83, 1-39.
Hatcher, R. A.
(1902) Am.Jour.Pharm., 74, 136.
Hatcher, W. H. and Skirrow, F. W.
(i9i7)J.Am.Chem.Soc.,39, 1939-1977.
v. Hauer.
(1858) J.prakt.Chem., 74, 433.
Hauser, O.
(1905) Z.anorg.Chem., 45, 194.
(1907) Z.anorg.Chem., 54, 196-212.
Hauser, O. and Wirth, F.
(1908) Z.anal.Chem., 47, 389.
(1909) J.prakt.Chem., [2] 79, 358-68.
(i9O9a) Z.angew.Chem., 22, 484.
(1912) Z.anorg.Chem., 78, 75-94.
Heath, W. P.
(1915) Privately Printed, Atlanta,
Ga.
Hehner, O. and Mitchell, C. A.
(1897) J.Am.Chem.Soc., 19, 40.
van der Heide.
(1893) Z. physik.Chem., 12, 418.
Heintz.
(1854) Pogg.Annalen, 92, 588.
Heise, G. W.
(1912) J.Phys.Chem., 16, 373.
Helff, A.
(1893) Z.physik.Chem., 12, 217.
Hellwig.
(1900) Z.anorg.Chem., 25, 166-183.
Hempel, W.
(1901) Z.angew.Chem., 14, 865.
Hempel, W. and Tedesco, H.
(1911) Z.angew.Chem., 24, 2469.
Henderson, W. N. and Taylor, H. S.
(1916) J.Phys.Chem., 20, 670.
Hendrixon, W. S.
(1897) Z.anorg.Chem., 13, 73.
Henkel, H.
(1905) Dissertation, Berlin.
(1912) Landolt & Bernstein's,
" Tabellen," 4th Ed., 602.
Henry.
(1884) Compt.rend., 99, 1157.
Herold, J.
(1905) Z.Elektrochem, n, 417.
Herrmann, Gottfried.
(1911) Z.anorg.Chem., 71, 257-302.
Herz, W.
(1898) Ber., 31, 2671.
(1900) Z.anorg.Chem., 25, 155.
(1902) Z.anorg.Chem., 30, 281.
(1903) Z.anorg.Chem., 33, 355.
(1903) Z.anorg.Chem., 34, 205.
(1905) Dissertation (Berlin).
(1910) Z.anorg.Chem., 68, 69, 165.
(i9ioa) Z.anorg.Chem., 66, 93, 358.
(19100) Z.anorg.Chem., 65, 341-4.
Herz, W.
(19100) Z.anorg.Chem., 67, 365.
(1911) Z.anorg.Chem., 70, 70, 170.
(191 la) Z.anorg.Chem., 71, 206.
(191 ib) Z.anorg.Chem., 72, 106.
(1911-12) Z.anorg.Chem., 73, 274.
(1917) Z.Elektrochem., 23, 23-4.
Herz, W. and Anders, G.
(1907) Z.anorg.Chem., 52, 164-72,
271-8.
Herz, W. and Bulla, A.
(1909) Z.anorg.Chem., 63, 282-4.
(1911) Z.anorg.Chem., 71, 255.
Herz, W. and Fischer, H.
(1904) Ber., 37, 4747.
(1905) Ber., 38, 1140.
Herz, W. and Knoch.
(1904) Z.anorg.Chem., 41, 319.
(1905) Z.anorg.Chem., 45, 263-8.
Herz, W. and Kuhn. F.
(1908) Z.anorg.Chem., 58, 159-67.
(1908) Z.anorg.Chem., 60, 152-62.
Herz, W. and Kurzer, A.
(1910) Z.Elektrochem.. 16, 240, 869.
Herz, W. and Lewy.
(1905) Z.Elektrochem., n, 818.
Herz, W. and Muhs, G.
(1903) Ber., 36, 3717.
Herz, W. and Paul, W.
(1913) Z.anorg.Chem., 82, 431.
(1914) Z.anorg.Chem., 85, 214.
Herz, W. and Rathmann, W.
(1913) Z.Elektrochem., 19, 553, 887.
Herzfeld.
(1892) Z.Ver.Zuckerind., 181.
(1897) Z.Ver.Zuckerind., 34, 820.
von Hevesy, Geo.
(1900) Z.physik.Chem., 73, 537.
(1909) Z.Elektrochem., 15, 529.
(1911) Phys.Ztschr., 12, 1214.
(1912) J.Phys.Chem., 16, 429.
von Hevesy, G. and Rona, E.
(1915) Z.physik.Chem., 89, 303.
Hicks, W. B.
(1915) J.Am.Chem.Soc., 37, 844.
Hildebrand, J. H., Ellefson, E. T. and
Beebe, C. W.
(1917) J.Am.Chem.Soc., 39, 2302.
Hill, A. E.
(1908) J.Am.Chem.Soc., 30, 68-74.
(1917) J.Am.Chem.Soc., 39, 218-31.
Hill, A. E. and Simmons, J. D.
(1909) J.Am.Chem.Soc., 31, 821-39.
(1909) Z.physik.Chem., 67, 594-617.
Hill, A. E. and Zink, W. A. H.
(1909) J.Am.Chem.Soc., 31, 44.
Hill, C. A. and Cocking, T. T.
(1912) Pharm.Jour.(Lond.), 89, 155.
Hill, J. Rutherford.
(1900) Pharm.Jour.(Lond.), 64, 185.
Hilpert, S.
(1916) Z.angew.Chem., 29, I, 57-9.
(1916) Chem.Abs., 10, 1924.
798
AUTHOR INDEX
Hinrichsen, F. W. and Sachsel, E.
(1904-05) Z.physik.Chem., 50,81-99.
His, W. Jr. and Paul, T.
(1900) Z.physiol.Chem., 31, 1-42,
64-78.
Hissink, D. J.
(1900) Z.physik.Chem., 32, 557.
Hitchcock, F. R. M.
(1895) J.Am.Chem.Soc., 17, 529.
van't Hoff, J. H.
(1901) Sitzber.k.Akad.Wiss. (Berlin),
P- 1035.
(1905) Z.anorg.Chem., 47, 247.
(1912) " Untersuchungen iiber die
Bildungsverhaltnisse der
Ozeanischen Salzablager-
ungen, inbesondere des
Staasfurter Salzlagers."
von J. H. van't Hoff et al
Herausgegeben von H.
Precht & E. Cohn.
(Leipzig, 1912).
van't Hoff, J. H. and Goldschmidt, H.
(1895) Z.physik.Chem., 17, 508.
van't Hoff, J. H. and Meyerhofifer, W.
(1898) Z.physik.Chem., 27, 75.
(1899) Z.physik.Chem., 30, 64-88.
van't Hoff, J. H. and Kenrick, F. B.
(1912) " Ozeanischen Salzablagerun-
gen," pp. 37-40.
Hoffmann, Fr. and Langbeck, K.
(1905) Z.physik.Chem., 51, 303, 393,
412.
Hofmann, K. A., Hobold, K. and Quoos.
(1911-12) Liebig's Ann., 386,304-
3!7-
Hofmann, K. A. and Hobold, K.
(1911) Ber., 44, 1776.
Hofmann, K. A,, Kirmireuther, K. and
Thai, A.
(1910) Ber., 43, 188.
Hofman, K. A., Roth, R., Hobold, K.
and Metzler, A.
(1910) Ber., 43, 2628.
Hoglund, A. T.
(1912) Z.Ver.Zuckerind., 1118-1127.
Hoitsema, C.
(1895) Z.physik.Chem., 17, 651.
(1898) Rec.trav.chim., 17, 310.
(18983) Z.physik.Chem., 27, 315.
Holde, D.
(1910) Z.Elektrochem., 16, 442.
Holland, A.
(1897) Ann. chim. anal., 2, 243.
Holleman, A. F.
(1893) Z.physik.Chem., 12, 135.
(1896) Rec.trav.chim. 15, 159.
(1898) Rec.trav.chim. 17, 247, 324.
(1910) Rec.trav.chim. 29, 396.
(1913) Rec.trav.chim.
(1914) Rec.trav.chim.
136.
6-29.
Holleman, A. F. and van den Arend, J. E.
(1909) Rec.trav.chim., 28, 411.
Holleman, A. F. and Antusch, A. C.
(1894) Rec.trav.chim., 13, 293.
Holleman, A. F. and de Bruyn, B. R.
(1900) Rec.trav.chim., 19, 83, 191,
365.
Holleman, A. F. and Caland, P.
(1911) Ber., 44, 2506.
Holleman, A. F., Hartogs, J. C., and
van der Linden, T.
(1911) Ber., 44, 705.
Holleman, A. F. and Huisinga, J.
(1908) Rec.trav.chim., 27, 275.
Holleman, Kohlrausch and Rose.
(1893) Z.physik.Chem., 12, 129,
241.
Holleman, A. F. and van der Linden, T.
(1911) Rec.trav.chim., 30, 318.
Holleman, A. F. and Pollak, J. J.
(1910) Rec.trav.chim., 29, 429.
Holleman, A. F. and Rinkes, I. J.
(1911) Rec.trav.chim., 30, 55.
Holleman, A. F. and Sluiter, C. H.
(1906) Rec.trav.chim., 25, 212.
Holleman, R.
(1903) Z.physik.Chem., 43, 129-159.
(1905-06) Z.physik.Chem., 54, 98-
no.
Holmberg, O.
(1907) Z.anorg.Chem., 53, 83-134.
Holt, A. and Bell, N. M.
(1914) J.Chem.Soc.(Lond.), 105, 633.
Holty, J. G.
(1905) J.Phys.Chem., 9, 764.
Homfray, I. F.
(1910) J.Chem.Soc.(Lond.),97, 1669.
Hooper.
(1882) Pharm.J.(Lond.), [3], 13, 258.
Horiba, S.
(191 1-12) Mem.Coll.Sci.Eng.(Kyoto),
3, 63-78.
(1914-16) Mem.Coll.Sci. (Kyoto), I,
Horn, D. W.
(1907) Am.Chem.Jour., 37, 471.
Horn, D. W. and Van Wagener.
(1903) Am.Chem.Jour., 30, 347.
Houston and Trichborne.
(1890) Brit.Med.Jour., 1063.
Howe, Jas. L.
(1894) J.Am.Chem.Soc., 16, 388.
Hudson, C. S.
[1904) J.Am.Chem.Soc., 26, 1072.
'1908) J.Am.Chem.Soc., 30, 1767-83.
Hudson, C. S. and Yanovsky, E.
(1917) J.Am.Chem.Soc., 39, 1037.
Huecke.
(1884) J.prakt.Chem., [2], 29, 49.
Hiifner, G.
(1895) Archiv.anat.u.physiol., 209-
212.
(1906-07) Z.physik.Chem., 57, 615-
622.
(1907) Z.physik.Chem., 59, 416.
799
AUTHOR INDEX
Hiifner, G. and Kulz.
(1895) J.prakt.Chem., 28, 256.
Hulett, G. A.
(1901) Z.physik.Chem., 37, 406.
Hulett, G. A. and Allen, L. E.
(1902) J.Am.Chem.Soc., 24, 674.
Hunt.
(1870) Am.Jour.Sci., [2], 40, 154.
Hiittig, Gustav, F.
(1914) Z.physik.Chem., 87, 144. *
Ulingworth, B. and Howard, A.
(1884) Phil.Mag., [5], 18, 124.
Imadsu, A.
(1911-12) Mem.Coll.Sci.Eng. (Ky-
oto), 3, 257-63-
Inglis, J. K. H.
(1903) J.Chem.Soc.(Lond.), 83, 1010.
Irving and Young.
(1888) J.Chem.Soc.(Lond.), 56, 344.
Isaac, Florence.
(1908) J.Chem.Soc.(Lond.), 93, 398,
927.
(1910) Proc.Roy.Soc.(Lond.), 84, A,
348.
(1913) Proc.Roy.Soc.(Lond.), 88,205.
van Itallie, E. J.
(1908) Z.anorg.Chem., 60, 358-65.
van Iterson-Rotgans, J. W.
(1913) Chem.Weekblad., 10, 920-37.
(1914) Z.physik.Chem., 87, 305.
Iwaki, J.
(1914) Mem.Coli.Sci.(Kyoto), i, 81-8.
Iwig and Hecht.
(1886) Liebig's Ann., 233, 167.
Jackson, R. F.
(1914) J.Am.Chem.Soc., 36, 2350.
(1914) Bull.BureauStandards, 2, 331-
Jacobs, W. 34'
(1917) Chem.Weekblad., 14, 208-12.
Jacobson, C. A. and Holmes, A.
(1916) J.Biol.Chem., 25, 29-53.
Jaeger, A.
(1901) Z.anorg.Chem., 27, 25.
Jaeger, F. M.
(1904) Z.Kryst.Min., 38, 583.
(1905) Proc.k.Akad.Wet.(Amst.), 7,
665.
(1906) Proc.k.Akad.Wet.(Amst.)f 8,
618.
(1907) Z.Kryst.Min., 42, 236-76.
(1907) Rec.trav.chim., 26, 329.
(1908) Proc.k.Akad.Wet.(Amst.), 436.
(1912) 8th Int.Cong.Appl.Chem., 2,
139-
Jaeger, F. M. and Doornbosch, H. J. D.
(1912) Z.anorg.Chem., 75, 261.
Jaeger, F. M. and van Klooster, H. S.
(1912) Z.anorg.Chem., 78, 245.
Jaeger, F. M. and van Kregten, J. R. N.
(1912) Proc.k.Akad.Wet.(Amst.), 14,
733.
Jaeger, F. M. and Menke, J. B.
(1912) Z.anorg.Chem., 75, 241-260.
(1912) Proc.k.Akad.Wet.(Amst.), 14,
724.
Jaenecke, E.
(1908) Z.physik.Chem., 64, 343.
(1912) Z.physik.Chem., 80, I.
Jakowkin, A. A.
(1895) Z.physik.Chem., 18, 588.
(1896) Z.physik.Chem., 20, 38.
(1899) Z.physik.Chem., 29, 630.
James, C. and Holden, H. C.
(1913) J.Am.Ch,em.Soc., 35, 559.
James, C. and Pratt, L. A.
(1910) J.Am.Chem.Soc., 32, 873.
James, C. and Robinson, J. E.
(1913) J.Am.Chem.Soc., 35, 754.
James, C. and Whittemore, C. F.
(1912) J.Am.Chem.Soc., 34, 1168.
James, C., Whittemore, C. F. and
Holden, H. C.
(1914) J.Am.Chem.Soc., 36, 1854.
James, C. and Willand, P. S.
(1916) J.Am.Chem.Soc., 38, 1499.
Jantsch, G.
(1912) Z.anorg.Chem., 76, 321.
Jantsch, G. and Griinkraut, A.
(1912-13) Z.anorg.Chem., 79, 309-
321.
Jaques, A.
(1910) Trans.FaradaySoc., 5, 235.
Jarry, R.
(1897) Compt.rend., 124, 288-91.
(1899) Ann.chim.phys., [7], 17, 342.
Jellinek, K.
(1911) Z.anorg.Chem., 70, 86-134.
Jensen, H. R.
(1913) Pharm.Jour.(Lond.), 90, 658-
60.
Jo, Inohiko.
(1911) Mem. coll. sci.Eng. (Kyoto), 3,
41-9, 212.
(1912) Tokyo Chem.Soc., 33, No. 7,
July.
Joannis, A.
(1882) Ann.chim.phys., [5], 26, 489.
(1906) Ann.chim.phys., [8], 7, 41.
Johnson.
(1886) Chem.News., 54, 75.
Johnston, J.
(1915) J.Am.Chem.Soc., 37, 2001-
2020.
Johnston, J. and Williamson, E. D.
(1916) J.Am.Chem.Soc., 38, 975-83.
Jolin.
(1889) Arch.anat.u.physiol., 262.
Jones, B. M.
(1908) J.Chem.Soc.(Lond.), 93, 1744.
Jones, Grinnel, and Hartman, M. L.
(1915) J.Am.Chem.Soc., 37, 241.
(1916) Trans. Am. Electrochem.Soc.,
30, 295-326.
800
AUTHOR INDEX
Jones, H. C.
(1907) Carnegie Publication No. 60,
Washington, D.C.
Jones, H. O.
(1907-98) Proc. Cambridge Phil.Soc.,
14, 27-9.
Jones, W. J.
(1911) J.Chem.Soc.(Lond.), 99, 392.
de Jong, A. W. K.
(1909) Rec.trav.chim., 28, 343.
(1912) Rec.trav.chim., 31, 256.
Jb'rgensen.
20, 195.
30, i.
2J, 42, 208.
(1879) J.prakt.Chem.,
(1884) J.prakt.Chem.,
(1890) J.prakt.Chem.,
Joulin.
(1873) Ann.chim.phys., [4], 30, 260.
Journiaux, M.
(1912) Bull. soc.chim. (Paris), [4], u,
129, 516, 546-52.
Joyner, R. A.
(1912) Z.anorg.Chem., 77, 108.
Jungfleisch, E.
(1912) Compt.rend., 155, 801.
Jungfleisch, E. and Landrieu, Ph.
(1914) Ann.chim., 2, 1-56, 333.
(i9i4a) Compt.rend., 158, 1306-11.
Jiirgens.
(1885) Jahresber.Chem., 1722.
Just, G.
(1901) Z.physik.Chem., 37, 342-367.
Juttner, F.
(1901) Z.physik.Chem., 38, 56-75.
Kachler, M. J.
(1870) Bull. soc.chim., 13, 460.
Kahlenberg, L. and Brewer, R. K. .
(1908) J.Phys.Chem., 12, 283-9.
Kahlenberg, L. and Krauskopf, F. C.
(1908) J.Am.Chem.Soc., 30, 1104-15.
Kahlenberg, L. and Wittich, W. J.
(1909) J.Phys.Chem., 13, 421-5.
Kahlukow, I. and Sachanow, A.
(I9°9) J.Russ.Phys.Chem.Soc., 41,
1755-
Karandeeff, B.
(1909) Zentralbl.Min.Geol., p. 728.
(1910) Z.anorg.Chem., 68, 188.
Karl, G.
(1910) Z.anorg.Chem., 68, 57.
Karplus.
(1907) Dissertation, Berlin.
Landolt & Bornstein's " Tab-
ellen " 4th Ed., p. 563.
Karsten.
(1864-5) Ann.der Chem.u.Pharm.
Suppl.Bd., 3, 170.
Karsten, B. J.
(1907) Z.anorg.Chem., 53, 367.
Katz, S. H. and James, C.
(1913) J.Am.Chem.Soc., 35, 872.
Kendall, J.
(1911) Proc.Roy.Soc.(Lond.), A, 85,
200-19.
Kendall, J.
(1912) PJiil.Mag. [6], 23, 958.
(1914) J.Am.Chem.Soc., 36, 1722.
(i9i4a) J.Am.Chem.Soc., 36, 1222.
(1916) .Am.Chem.Soc., 38, 1309.
Kendall, J. and Booge, J. E.
(1916) .Am.Chem.Soc., 38, 1712.
Kendall, . and Carpenter, C. D.
(1914) .Am.Chem.Soc., 36, 2502.
Kendall, . and Gibbons, W. A.
(1915) J.Am.Chem.Soc., 37, 149.
Keppish.
• (1888) Monatsh.Chem., 9, 589.
Kernot, G., d'Agostino, E. and Pelle-
grino, M.
(1908) Gazz.chim.ital., 38, I, 532-54.
Kernot, G. and Pomilio, M.
(1912) Rend.accad.sci.fis.nat.(Nap-
oli), [3], 17, 353-8.
Ketner.
(1901-02) Z.physik.Chem., 39, 645.
Keyes, D. B. and Hildebrand, J. H.
(1917) J.Am.Chem.Soc., 39, 2129.
Keyes, D. B. and James, C.
(1914) J.Am.Chem.Soc., 36, 634.
King, Chas. A. and Narracott, P.
(1909) Analyst, 34, 436-8.
King, H. and Orton, K. P. J.
(1911) J.Chem.Soc.(Lond.),99, 1381.
King, Harold and Pyman, F. L.
(1914) J.Chem.Soc.(Lond.), 105,
1238-59.
Kirschner, A.
(1912) Z.physik.Chem., 79, 247.
Klaus.
(1905) Phys.Ztschr., 6, 820.
Klein, O.
(1912) Z.anorg.Chem., 74, 158.
Kleven.
(1872) Chem.Centralbl., 434.
Klobbie, E. A.
(1897) Z.physik.Chem., 24, 623.
van Klooster, H. S.
(1910-11) Z.anorg.Chem., 69, 122,
135-57.
(1912-13) Z.anorg.Chem., 79, 223-9.
(1917) J.Phys.Chem., 21, 513-18.
Klose, G.
( 1 907 ) Archi v. I nternat . Pharmacody-
namie et Therapie, 17,
459-63.
Knietsch, R.
(1901) Ber., 34, 4099.
Knopp.
(1904) Z.physik.Chem., 48, 97-108.
Knox, Joseph.
(1909) J.Chem.Soc.(Lond.), 95, 1760.
Kobayashi, M.
(1911-12) Mem. Coll. Sci.Eng. (Ky-
oto), 3, 218.
de Kock, A. C.
(1904) Z.physik.Chem., 48, 131.
801
AUTHOR INDEX
Kofler, M.
(1913) Monatsh.Chem., 34, 389.
(1913) Sitzber.k.Akad.Wiss.(Wien)
Abt., I la, 122, 1473-80.
Kohler.
(1879) Z.anal.Chem., 18, 242.
Kohler.
(1897) Z.Ver.Zuckerind., 47, 447.
Kohlrausch, Fr.
(1879) Wied.Ann., i.
(1891) Ber., 24, 3561.
(1891) Wied.Ann., 44, 577.
(1897) Sitzber.k.Akad.Wiss. (Berlin),
90.
(1903) Z.physik.Chem., 44, 197.
(1904-05) Z.physik.Chem., 50, 355-6.
(1908) Z.physik.Chem., 64, 121-69.
Kohlrausch, F. and Rose, F.
(1893) Z.physik.Chem., 12, 129, 135,
241.
Kohn, M.
(1909) Z.anorg.Chem., 63, 337-9.
Kohn, M. and O'Brien.
(1898) J.Soc.Chem.Ind., 17, 100.
Kohn, M. and Klein, A.
(1912) Z.anorg.Chem., 77, 254.
Kohnstamm and Cohn.
(1898) Wied.Ann., 65, 344.
Kohnstamm, Ph. and Timmermans, J.
(i9i3)Proc.k.Akad.Wet.(Amst.),i02i.
Kolb.
(1872) Bull.soc.ind.Mulhouse, 222.
de Kolossovsky, N.
(1911) Bull. soc.chim. (Paris), [4], 9,
632-7.
(1911) Bull.soc.chim.(Belg.), 25, 183,
235-
Kolthoff, I. M.
(1917) Chem.Weekblad., 14, 1081.
Konig.
(1894) Monatsh.Chem., 15, 23.
de Koninck, L. L.
(1907) Bull.soc.chim.(Belg.), 21, 141.
Konowalow, D.
(1898) Jour.Russ.Phys.Chem.Soc.,
W, 30, 367-
(1898) Chem.Zentralbl., II, 659.
(i899a) Jour. Russ. Phys.Chem.Soc.,
3i» 910-
(i899b) Jour.Russ.Phys.Chem.Soc.,
3i» 985.
(1900) Chem.Zentralbl., I, 646.
(igoob) Chem.Zentralbl., I, 938.
(1903) Ann.Phys.(Wied.), [41,10,375,
Koopal, S. A.
(1911) Dissertation, Leyden, p. 128.
(1911) "Tables annuelles," 2, 463.
Koppel, J.
(1901-02) Z.physik.Chem., 42, 8.
(1904) Z.anorg.Chem., 41, 377.
(1905) Z.physik.Chem., 52, 405.
(1906) Ber., 39, 3738.
Koppel, J. and Blumenthal, R.
(1907) Z.anorg.Chem., 53, 228-67.
Koppel, J. and Cahn, M.
(1908) Z.anorg.Chem., 60, 53-112.
Koppel- Gumpery.
(1905) Z.physik.Chem., 52, 413.
Koppel, J. and Holtkamp, H.
(1910) Z.anorg.Chem., 67, 274.
Koppel-Wetzel.
(1905) Z.physik.Chem., 52, 395.
Korreng, E.
(1914) Neues Jahrb.Min.Geol.(Beil
Bd.), 37, 51-124.
(1915) Z.anorg.Chem., 91, 194.
Krasnicki.
(1887) Monatsh.Chem., 8, 597.
Kremann, R.
(1904) Monatsh.Chem., 25, 1242-
1324.
(1905) Monatsh.Chem., 26, 143.
(1906) Monatsh.Chem., 27, 91-107,
125-80, 627.
(1907) Monatsh.Chem., 28, 8, 895,
1125.
(1908) Jahrber.k.geol.Reichsanstalt
(Wien), 58, 662.
(1909) "The Use of Thermic Analysis
for the Detection of Chemical
Compounds," Sammlung
Chem. u. Chem.-Techn. Vor-
trage,XIV,6-7, pp. 213-288
(F. Enke, Stuttgart).
(1910) Monatsh.Chem., 31, 843, 855.
(i9ioa) Monatsh.Chem., 31, 275.
(1911) Monatsh.Chem., 32, 609.
( ) Sitzber.k.Akad.Wiss.(Wien),
120, lib, 329.
Kremann, R. et al.
(1908) Monatsh.Chem., 29, 863-91.
Kremann, R. and Borjanovics, V.
(1916) Monatsh.Chem., 37, 59-84.
Kremann, R., Daimer and Beunesch.
(1911) Monatsh.Chem., 32, 620.
Kremann, R. and Ehrlich.
(1908) Jahrber.k.geol.Reichsanstalt
(Wien), 58, 569.
Kremann, R. and Hofmeier, F.
(1908) Monatsh.Chem., 29, mi.
(1910) Monatsh.Chem., 31, 201.
Kremann, R. and Huttinger, K.
( 1 908) Jahrber. k.Geol. Reichsanstalt
(Wien), 58, 637.
Kremann, R. and Janetzky, E.
(1912) Monatsh.Chem., 33, 1055-62.
Kremann, R. and Kerschbaum, F.
(1907) Z.anorg.Chem., 56, 218-22.
Kremann, R. and Klein, H.
(1913) Monatsh.Chem., 34, 1291.
Kremann, R. and Kropsch, R.
(1914) Monatsh.Chem., 35, 561, 823,
841.
Kremann, R. and Noss, F.
(1912) Monatsh.Chem., 33, 1205.
802
AUTHOR INDEX
Kremann, R. and Rodemund, H.
(1914) Monatsh.Chem., 35, 1065-
1086.
(1914) Z.anorg.Chem., 86, 373.
Kremann, R. and Rodinis, O.
(1906) Monatsh.Chem., 27, 125-180.
Kremann, R. and Schoulz, R.
(1912) Monatsh.Chem., 33, 1063,
1081.
Kremann, R. Wischo, F. and Paul, R.
(1915) Monatsh.Chem., 36, 915.
Kremann, R. and Zitek, A.
(1909) Monatsh.Chem., 30, 311-40.
Kremers.
(1852) Pogg.Ann., 85, 248.
(1854) Pogg.Ann., 92, 497.
(1855) Pogg.Ann., 94, 271; 95, 468.
1856) Pogg.Ann., 99, 47.
i856a) Pogg.Ann., 97, 5.
1858) Pogg.Ann., 103, 57, 133, 165.
(1858) Pogg.Ann., 104, 133.
(1860) Pogg.Ann., in, 60.
Kreusler and Herzhold.
(1884) Ber., 17, 34.
Krug, W. H. and Cameron, F. K.
(1900) J.Phys.Chem., 4, 188.
Krug, W. H. and McElroy, K. P.
(1892) J.Anal.Ch., 6, 184.
Krusemann, H. D.
(1876) Ber., 9, 1467.
Kriiss, G. and Nilson, L. F.
(1887) Ber., 20, 1696.
Kruyt, H. R.
(1908) Z.physik.Chem., 64, 513.
(1908-09) Z.physik.Chem., 65, 497.
(1912) Z.physik.Chem., 79, 667.
Krym, V.
(1909) J.Russ.Phys.Chem.Soc., 41,
382-5; Chem.Zentr., II, 68 1.
Kulisch.
(1893) Monatsh.Chem., 14, 567.
Kultascheff.
(1903) Z.anorg.Chem., 35, 187.
Kumpf.
(1882) Wied.Ann.Beibl., 6, 276.
Kunheim and Zimmerman.
(1884) Dingler.polyt.J., 252, 478.
Kunschert, F.
(1904) Z.anorg.Chem., 41, 338.
Kuriloff, B.
(1897) Z.physik.Chem., 24, 441-467.
(i897a) Z.physik.Chem., 23, 93, 547,
673.
(1898) Z.physik.Chem., 25, 419-440.
Kurnakov, N. S. and Efrenov, N. N.
(1912) Jour.Russ.Phys.Chem.Soc.,
44, 1992-2000.
(1912) Ann.Inst.Polyt.(Petrograd),
18, 105.
Kurnakov, J., Krotkov, D. and Oksman,
M.
(1915) Jour.Russ.Phys.Chem.Soc.,
47, 558-88.
Kurnakov, H. and Kviot, I.
(1913) Ann.Inst.Polyt.(Petrograd),
20, 664.
Kurnakov, N. S. and Solovev, V.
(1916) J.Russ.Phys.Chem.Soc., 48,
1338.
Kurnakov, N. S. and Wrzesnewsky,
J. B.
(1912) Z.anorg.Chem., 74, 89.
Kurnakov, N. S. and Zemcznzny.
(1907) Z.anorg.Chem., 52, 186.
Kiister, F. W.
(1890) Z.physik.Chem., 5, 601.
(1891) Z.physik.Chem., 8, 577.
(1895) Z.physik.Chem., 17, 357.
Kiister, F. W. and Dahmer, Geo.
(1905) Z.physik.Chem., 51, 240.
Kiister, F. W. and Heberlein, E.
(1905) Z.anorg.Chem., 43, 56.
Kiister, F. W. and Kremann, R.
(1904) Z.anorg.Chem., 41, 19,
Kiister and Thiel.
(1899) Z.anorg.Chem., 21, 116.
(1903) Z.anorg.Chem., 33, 139.
Kiister, F. W. and Wiirfel, Walter.
(1904-5) Z.physik.Chem., 50, 70.
van der Laan, F. H.
(1907) Rec.trav.chim., 26, 29.
Lachaud, M. and Lepierre, C.
(1891) Bull.soc.chim., [3], 6, 230-5.
Ladenburg, A.
(1902) Ber., 35, 1256.
Ladenburg, A. and Doctor, G.
(1899) Ber., 32, 50.
Ladenburg, A. and Herz, W.
(1898) Ber., 31, 937.
Ladenburg, A. and Sobecki.
(1910) Ber., 43, 2375.
Lai De, R.
(1917) J.Chem.Soc.(Lond.), in, 55.
Lami, Pio.
(1908) Chem.Zentr., II, 755.
(1908) Boll. chim. farm., 47, 435-441.
Lamouroux, F.
(1899) Compt.rend., 128, 998.
Lamy.
(1863) Ann.chim.phys., [3], 67, 408.
(1878) Ann.chim.phys., [5], 14, 145.
Landau, M.
(1893) Monatsh.Chem., 14, 712.
(1910) Z.physik.Chem., 73, 200-11.
Landolt and Bprnstein.
(1912) Physikalisch-Chemische Tab-
ellen, 4th Ed.
Langheld, K. and Oppmann, F.
(1912) Ber., 45, 3753.
Lassaigne.
(1876) J.chim.med., 12, 177.
von Laszczynski, St.
(1894) Ber., 27, 2285.
Laurie, A. P.
(1912) Proc.Roy.Soc.(Edin.), 31,388.
AUTHOR INDEX
Lautz, H.
(1913) Z.physik.Chem., 84, 633.
Laws, E. G. and Sidgwick, N. V.
(1911) J.Chem.Soc.(Lond.), 99, 2088.
Leather, J. W. and Mukerji, J. M.
(1913) Mem. Dept.Agr. (India), Chem.
Sen, 3, 177-204.
Leather, J. W. and Sen, J. N.
(1909) Mem. Dept.Agr. (India), Chem.
Sen, i, 117-131.
(1914) Mem. Dept.Agr. (India), Chem.
Sen, 3, 205-34.
Lebeau, P.
(1906) Ann.chim.phys., [8], 9, 482-4.
(1911) Compt.rend., 152, 440.
Lebedew, P.
(1911) Z.anorg.Chem., 70, 302, 316.
LeBlanc, M. and Novotny, K.
(1906) Z.anorg.Chem., 51, 181-201.
LeBlanc, M. and Noyes, A. A.
(1890) Z.physik.Chem., 6, 386.
LeBlanc, M. and Schmandt, W.
(1911) Z.physik.Chem., 77, 621-30.
Lecat.
(1909) These, Brussels.
LeChatelier.
(1894) Compt.rend., 118, 350, 709,
800.
(1897) Compt.rend., 124, 1094.
de Leeuw, H. L.
(1911) Z.physik.Chem., 77, 311.
van Leeuwen, J. Docters.
(1897) Z.physik.Chem., 23, 44.
Lefort.
(1878) Ann.chim.phys., [5], 15, 326.
Lehmann, M.
(1914) Chem.Ztg., 38, 389, 402.
Leidie.
(1882) Compt.rend., 95, 87.
(1890) Compt.rend., in, 107.
Lenher, V. and Merrill, H. B.
(1917) J.Am.Chem.Soc., 39, 2630.
Leopold, G. H.
(1909) Z.physik.Chem., 66, 361.
(1910) Z.physik.Chem., 71, 51.
Lepierre, C. and Lachaud, M.
(1891) Compt.rend., 113, 196.
Lespieau.
(1894) Bull.soc.chim., [3], n, 72.
Levi, M. G.
(1901) Gazz.chim.ital., 31, II, 523.
(1902) Z.physik.Chem., 41, no.
Levi-Malvano, M.
(1906) Z.anorg.Chem., 48, 446.
(1905) Atti accad.Lincei, [5], 14, II,
502-10.
Lewis, G. N. and Burrows, G. H,
(1912) J.Am.Chem.Soc., 34, 1525.
Lewis, G. N. and Storch, H.
(1917) J.Am.Chem.Soc., 39, 2551.
Lewis, W. K.
(1914) J.Ind.Eng.Chem., 6, 308.
Ley, H. and Heimbuchen.
(1904) Z.Elektrochem., 10, 303.
Ley, H. and Schaefer, K.
(1906) Ber., 39, 1263.
Lichty, D. M.
(1903) J.Am.Chem.Soc., 25, 474.
Lidoff.
(1893) Bull.soc.chim., [3], 10, 356.
Lieben and Rossi.
(1871) Liebig's Ann., 159, 60.
Liebermann, C.
(1902) Ber., 35, 1094.
(1903) Ber., 36, 180.
. Limbosch, H.
(1909) Bull.soc.chim.Belg., 23, 179-
200.
Lincoln, A. T.
(1900) J.Phys.Chem., 4, 176.
(1904) J.Phys.Chem., 8, 251.
van der Linden, T.
(1912) Ber., 45, 237.
(1916) Arch.Suikerind, 24, 1113-28.
(1917) Chem.Abs., n, 3122.
Linebarger, C. E.
(1892) Am.Chem.Jour., 14, 380.
(1894) Am.Chem.Jour., 16, 214.
, (1895) Am.Jour.Sci., 49, 48-53-
Lindner, J.
(1912) Monatsh.Chem., 33, 645.
Linhart, G. A.
(1915) J.Am.Chem.Soc., 37, 258-274.
Little, W. G.
(1909) Biochem.Jour., 4, 30.
Lloyd, S. J.
(1918) J.Phys.Chem., 22, 300-3.
Locke.
(1901) Am. Chem. J., 26, 174.
(1902) Am.Chem.J., 27, 459.
Loewel.
(1851) Ann.chim.phys., [3], 33, 382.
(1855) Ann.chim.phys., [3], 43, 413.
Long.
(1888) J.Anal.Chem., 2, 243.
Longi.
(1883) Gazz.chim.ital., 13, 87.
Longuimine.
(1862) Liebig's Ann., 121, 123.
Lord, R. C.
(1907) J.Phys.Chem., u, 182.
Lorenz, R., Jabs, A. and Eitel, W.
(1913) Z.anorg.Chem., 83, 39.
Lorenz and Ruckstuhl.
(1906) Z.anorg.Chem., 51, 70.
Lothian, J.
(1909) Pharm.Jour.(Lond.), 82, 292.
Louise, E.
(1909) Compt.rend., 149, 284-6.
(1911) J.pharm.chim., [7], 3, 377-385-
(1911) J.pharm.chim., [7], 4, 193-7 •
(1911) Ann.fals., 4, 302-5.
Lowel.
(1851) Ann.chim.phys., [3], 33, 3«2.
804
AUTHOR INDEX
Lb'wenherz, R.
(1894) Z.physik.Chem., 13, 479.
(1895) Z.physik.Chem., 18, 82.
(1898) Z.physik.Chem., 25, 395-410.
Lubarsch.
(1889) Wied.Ann.Physik., [2], 37, 525.
Lubavin.
(1892) J.Russ.Ph^ Chem.Soc., 24,
389.
de Lucchi, G.
(1910) Russ.min., 32, 21.
(1910) "Tables annuelles, "1,381, 403.
Lumiere, A. and L. and Seyewetz, A.
(1902) Bull.soc.chim., [3], 27, 1213.
Lumsden, J. S.
(1902) J.Chem.Soc.(Lond.), 81, 355.
(1905) J. Chem.Soc. (Lond.), 89, 90.
Lunden, Harold.
(1905-6) Z.physik.Chem., 54, 564.
(1913) Medd.K.Vetenskapsakad.
Nobelinst., 2, No. 15.
(1913) Chem.Abs., 7, 2887.
Luther, R. and Leubner, A.
(1912) J.prakt.Chem., [2], 85, 314.
(i9i2a) Z.anorg.Chem., 74, 389.
Lutz, O.
(1902) Ber., 35, 2462.
(1910) Ber., 43, 2637.
van Maarseveen, G. (Goldschmidt, H.)
(1898) Z.physik.Chem., 25, 90-99.
Maass, O. and Mclntosh, D.
(1912) J. Am. Chem.Soc., 34, 1279.
(1913) J.Am.Chem.Soc., 35, 538.
Maben.
(1883-84) Pharm. Jour. (Lond.), [3],
14, 505-
MacAdam, D. J., Jr. and Pierle, C. A.
(1912) J.Am.Chem.Soc., 34, 604.
MacArthur, C. G.
(1916) J. Phys.Chem., 20, 495.
McBride, R. S.
(1910) J. Phys.Chem., 14, 189-200.
McCaughey, W. J.
(1909) J.Am.Chem.Soc., 31, 1261.
McCoy, H. N. and Smith, H. J.
(1911) J.Am.Chem.Soc., 33, 468-473.
McCoy, H. N. and Test, Chas. D.
(1911) J.Am.Chem.Soc., 33, 473-6.
McCrae, J. and Wilson, W. E.
(1903) Z.anorg.Chem., 35, n.
M'David, J. W.
(1909-10) Proc.Roy.Soc. (Edin-
burgh), 30, 440-7.
McDaniel, A. S.
(1911) J. Phys.Chem., 15, 587-610.
McDermott, F. Alex.
(1911) J.Am.Chem.Soc., 33, 1963.
McDonnell, C. C. and Smith, C. M.
(1916) J.Am.Chem.Soc., 38, 2366.
Mclntosh, D.
(1903) J. Phys.Chem., 7, 350.
Mackenzie.
(1877) Wied.Ann.Physik., [2], I, 450.
McLauchlan, W. H.
(1903) Z.physik.Chem., 44, 600-633.
Maclaurin.
(1893) J.Chem.Soc.(Lond.), 63, 729.
Magnanini, G.
(1901) Gazz.chim.ital., 31, II, 542.
Magnier.
(1875) Bull.soc.chim., [2], 23, 483.
von Mailfert.
(1894) Compt.rend., 119, 951.
Maigret.
(1905) Bull.soc.chim. [3], 33, 631.
Mallet.
(1897) Am.Chem.Jour., 19, 807.
Malvano, L.
(1906) Z.anorg.Chem., 48, 446.
Malvano, L. and Mannino.
(1908) Atti accad.Lincei, [5], 17, II,
484.
Mameli, E. and Mannessier, A.
(1913) Gazz.chim.ital., 43, II, 594.
Manchot and Zechentmayer.
(1906) Liebig's Ann., 350, 368.
Mandelbaum, R.
(1909) Z.anorg.Chem., 62, 370-82.
Manuelli, A.
(1916) Ann.chim.applicata, 5, 13-24.
Mar.
(1892) Am.J.Sci., [3], 43, 521.
Marc, R.
(1906) Z.anorg.Chem., 48, 425.
(1907) Z.anorg.Chem., 53, 301.
Marchionneschi, M.
(1907) Apoth.Ztg., 22, 544.
(1907) Boll.chim.farm., 387.
Marckwald, W.
(1902) Ber., 35, 1599.
(1904) Ber., 37, 1041.
Harden,
(1914) !
(1916) ;
Marden,
(1916) .
(1917) .
W.
.Ind.Eng.Chem., 6, 315-20.
.Am.Chem.Soc.,
W. and Dover,
310.
ary V.
.Am.Chem.Soc., 38, 1239.
.Am.Chem.Soc., 39, 4.
Marie, C. and Marquis, R.
(1903) Compt.rend., 136, 684.
Marignac.
(1853) Ann.chim.phys., [3], 39, 184.
(1861) J.prakt.Chem., 83, 202.
(1866) Ann.chim.phys., [4], 8, 65.
Marino.
(1905) Gazz.chim.ital., 35, II, 351.
Markwald.
(1899) Ber., 32, 1089.
Marsh, J. E. and Struthers, R. de J. F.
(1905) J.Chem.Soc.(Lond.), 87, 1879.
Marshal, A.
(1906) J. Chem.Soc. (Lond.), 89, 1381.
Marshall.
(1891) J. Chem.Soc. (Lond.), 59, 771.
Marshall, H. and Bain, D.
(1910) J. Chem.Soc. (Lond.), 97, 1074-
1085.
805
AUTHOR INDEX
Marshall, H. and Cameron, A. T.
(1907) J.Chem.Soc.(Lond.), 91, 1522.
Mascarelli, L.
(1906) Atti accad.Lincei, [5], 15, I,
192; II, 459.
(I9o6a) Atti accad.(Lincei), [5], 15,
192.
(I9o6a) Gazz.chim.ital., 36, II, 880-
893.
(1908) Atti accad.Lincei, [5], 17, I,
29.
(1909) Gazz.chim.ital., 39, I, 251-84.
Mascarelli, L. and Ascoli, U.
(1907) Gazz.chim.ital., 37, I, 125.
Mascarelli, L. and Constantino, A.
(1909) Atti accad.Lincei, [5], 18, II,
104.
(1910) Gazz.chim.ital., 40, I, 41.
Mascarelli, L. and Pestalozza, U.
(1907) Atti accad. Lincei, [5],i6, II,
574-
(1908) Gazz.chim.ital., 38, I, 51.
(1908) Atti accad.Lincei, [5], 17, I,
601-9.
(1909) Gazz.chim.ital., 39, I, 218-
231.
Mascarelli, L. and Sanna, G.
(1915) Atti accad.Lincei, [5], 24, II,
94-
Massink, A.
(1916) Z.physik.Chem., 12, 351-80.
(1917) Chem.Weekblad., 14, 756.
Massol and Maldes.
(1901) Compt.rend., 133, 287.
Masson, I.
(1912-13) Proc.Roy.Soc.(Edin.), 33,
64-8.
Masson, J. J. Orme.
(1911) J.Chem.Soc.(Lond.), 99, 1132.
(1912) J.Chem.Soc.(Lond.) 101, 103.
Mathers, F. C. and Schluederberg, C. G.
(1908) J.Am.Chem.Soc., 30, 211.
Mathews, J. H. and Benger, E. B.
(1914) J.Phys.Chem., 18, 264.
Mathews, J. H. and Ritter, P. A.
(1917) J.Phys.Chem., 21, 269-74.
Mathews, J. H. and Spero, S.
(1917) J.Phys.Chem., 21, 402-6.
Matignon, C.
(1906) Ann.chim.phys., [8], 8, 249,
388, 407. *
(1909) 7th Internat.Cong.Appl.
Chem., 2, 53-57-
(igoga) Compt.rend., 148, 550.
Matteoschat, A.
(1914) Z.ges.Schiess.u.Sprengstoffw.,
9, 105-6.
Matthes, F.
(1911) Neues Jahrb.Min.Geol. (Beil.
Bd.), 31, 342-85-
Maumee.
(1864) Compt.Fend., 58, 81.
Mayer.
(1856) Liebig's Ann., 98, 193.
Mayer, O.
(1903) Ben, 36, 1741.
Mazatto.
(1891) Nuovo.cimento, [3], 29, 21.
Meerburg, P. A.
(1902) Z.physik.Chem. 40, 647.
(1903) Z.anorg.Chem., 37, 203.
(1904) Chem.Weekblad., i, 474.
(1905) Z.anorg.Chem., 45, i, 324.
(1908) Z.anorg.Chem., 59, 136-42.
(1909) van Bemmlen Festschrift, pp.
356-60.
(1911) Chem.Zentralbl., I, 1036.
Meerum-Terwogt.
(1905) Z.anorg.Chem., 47, 203.
Mees, C. E. K. and Piper, C. W.
(1912) Photogr.Jour., 33, 227.
Phot ogr. Jour., 36, ?H-
Photogr.Jour., 52, 2^1-37.
Meineke.
(1891) Liebig's Ann., 261, 360.
Melcher, A. C.
(1910) J.Am.Chem.Soc., 32, 50-66.
Meldrum, R.
(1913) Chem.News., 108, 199.
Mellor, J. W.
(1901) J.Chem.Soc.(Lond.), 79, 225.
Meneghini, D.
(1912) Gazz.chim.ital., 42, II, 474.
Menge, Otto.
(1911) Z.anorg.Chem., 72, 169-218.
Menke, J. B.
(1912) Z.anorg.Chem., 77, 283.
Menschutkin, B. N. (see pp. 379 and
39i).
(i905)Mem.St.PetersburgPolyt.Inst.,
4, 75-101.
(1906) Mem.St. Petersburg Polyt.Inst.,
5, 355-388.
(1907) Z.anorg.Chem. 52, 9, 155; 53,
26.
(i907a) Z.anorg.Chem., 54, 89-96.
(i9o8)Mem.St. Petersburg Polyt.Inst.,
9, 200-222.
(i909)Mem.St. Petersburg Polyt.Inst.,
n, 261, 567; 12, i.
(1909) Z.anorg.Chem., 61, 106, 113.
(19 1 o) Mem.St. Petersburg Polyt.Inst.,
13,1,263,411,565; 14,251.
(191 i)Mem.St. Petersburg Polyt.Inst.,
15* 65, 397, 613, 647, 757.
(i9i2)Mem.St. Petersburg Polyt.Inst.,
16, 33, 397-
L. W. C. and Dutt, N. N.
Menzies, A.
(1911) J.Am.Chem.Soc., 33, 1266.
Menzies, A. W. C. and Humphrey, E.G.
(1912) 8th Int. Congr.Appl. Chem., 2,
175-8.
Menzies, A. W. C. and Potter, P. D.
(1912) J.Am.Chem.Soc., 34, 1452.
806
AUTHOR INDEX
Merriman, R. W.
(1913) J.Chem.Soc.(Lond.), 103,1774.
Mescherzerski.
(1882) Z.anaLChem., 21, 399.
Metzner.
(1894) Compt.rend., 119, 683.
van Meurs, C. J.
(1916) Z.physik.Chem., 91, 313-46.
Meusser, A.
(1902) Ber., 35, 1303, 1422.
(1905) Z.anorg.Chem., 44, 80.
Meyer, J.
(1909) Z.Elektrochem., 15, 266.
(1911) Ber., 44, 2969.
Meyer, H, von.
(1901) Archiv.exp.Pathol.u.Pharma-
kol., 46, 334.
(1909) 7th Int. Cong. Appl. Chem.
Sec., 4, A2, 44.
Meyer, Hans von and Beer, R.
(1913) Monatsh.Chem., 34, 1202.
Meyer, Hans von, Brod, L. and
Soyka, W.
(1913) Monatsh.Chem., 34, 1125.
Meyer, R. J.
(1914) Z.anorg.Chem., 86, 285.
Meyer, Victor.
(1875) Ber., 8, 998.
Meyerhoffer, W.
(1904) Landolt and Bornstein "Tab-
ellen," 4th Ed., 1912, p. 486.
(1905) Z.physik.Chem., 53, 513-603.
(1912) Landolt and Bornstein "Tab-
ellen," 4th Ed., p. 481.
Meyerhoffer, W. und Saunders.
(1899) Z.physik.Chem., 28, 466; 31,
382.
Michael, Arthur.
(1901) Ber., 34, 3641, 3656.
Michael, Arthur and Garner, W. W.
(1903) Ber., 36, 904.
Michel and Kraft.
(1854) Ann.chim.phys., [3], 41, 471.
(1858) Ann.chim.phys., [3], 41, 478.
Miczynski, Z. N.
(1886) Monatsh.Chem., 7, 255-72.
Middelberg, W.
(1903) Z.physik.Chem., 43, 305-353.
Miers, H. A. and Isaac, F.
(1907) Proc.Roy.Soc.(Lond.), 79, A,
332.
(1908) Trans. Roy.Soc.(Lond.), 209,
A, 364-
(i9o8a) J.Chem.Soc.(Lond.), 93, 931.
Milbauer, J.
(1912-13) J.prakt.Chem., [2], 87, 398.
Milikau, J.
(1916) Z.physik.Chem., 92, 59-80.
Miller, W. Lash and McPherson, R. H.
(1908) J.Phys.Chem., 12, 709.
Mills, W. H., Parker, H. V. and
Prowse, R. W.
(1914) J.Chem.Soc.(Lond.), 105,1541.
Mills, R. V. and Wells, R. C.
(1918) Bull.U.S.Geol.Sur/ey, No.
693, P- 72.
Miolati, A.
(1892) Z.physik.Chem., 9, 651.
Mjtscherlich.
(1832) Pogg.Ann., 25, 301.
Moissan, H.
(1882) Bull.soc.chim., [2], 37, 296.
(1885) Ann.chim.phys., [6], 4, 136.
Moissan, H. and Siemens, F.
(1904) Compt.rend., 138, 657, 1300.
(1904) Bull.soc.chim., [3], 31, 1010.
(1904) Ber., 37, 2088.
Moles, E. and Jimeno, E.
(1913) Anales.soc.espan.fis.quim., II,
393-
Moles, E. and Marquina, M.
(1914) Anales.soc.espan.fis.quim., 12,
383-93.
Monkemeyer.
(1906) NJahrb.Min.Geol.(Beil.Bd.),
22, I.
Moody, G. T. and Leyson, L. F.
(1908) J.Chem.Soc.(Lond.), 93, 1767.
Moore, B. and Roaf, H. E.
(1904) Proc.Roy.Soc.(Lond.), 73,
382-412.
Moore, B., Wilson, F. P. and Hutchin-
son, L.
(1909) Biochem.Jour., 4, 347.
Moore, T. S. and Winmill, T. F.
(1912) J. Chem. Soc.(LoncL), 101,1662.
Morey, Geo. W.
(1917) J.Am.Chem.Soc., 39, 1173-
1229.
Morgan, J. L. R. and Benson, H. K.
(1907) J.Am.Chem.Soc., 29, 1176.
(1907) Z.anorg.Chem., 55, 356.
Morgan, J. C. and James, C.
(1914) J.Am.Chem.Soc., 36, 10-16.
Morell, R. S. and Hanson, E. K.
(1904) J.Chem.Soc.(Lond.), 85, 1520.
Morse, H.
(1902) Z.physik.Chem., 41, 708-734.
Moser, L.
(1909) Z.anorg.Chem., 61, 384.
Moufgang, E.
(1911) Wochschr.Brau., 28, 434-6.
(1911) J.Soc.Chem.Ind., 30, 1210.
Much in, G.
(1913) " Solubility of Calcium Iodide
in Organic Solvents," Pamphlet,
45 pp. and 12 charts, Kharkoff,
1913. (Reprint in the Russian
language received from author.)
See also Trav.sco.sci. physic.
Chem.Univ. Kharkoff 39 fasc.,
24, 1-49, I9I3-
Muir.
(1876) J.Chem.Soc.(Lond.),29, 857.
807
AUTHOR INDEX
Mulder, G. J.
(1864) Scheikundige Verhandelingen
en Onderzoekingen, Vol. 3, Pt. 2,
Bijdragen tot de Geschiedenis
van Het Scherkungig Gebonden
Water, Rotterdam, 1864.
Mulder, Gay-Lussac, Etard.
- (1894) Ann.chim.phys., [7], 2, 528.
MueUer, J. H.
(1917) J.Biol.Chem., 30, 39~4O.
Mueller, P. and Abegg, R.
(1906) Z.physik.Chem., 57, 514.
Miiller, C.
(1910) NJahrb.Min.Geol.(Beil.Bd.),
30, i.
(1912-13) Z.physik.Chem., 81, 483-
503.
Miiller.
(1887) Compt.rend., 104, 992.
(1889) Wied.Ann.Physik., [2], 37, 29.
(1892) Ann.chim.phys., [6], 27, 409.
Miiller, H.
(1912) J.Chem.Soc.(Lond.), 101,2400.
Muller, W.
(1903) Apoth.Ztg., 18, 208, 249, 257.
Muraro, F.
(1908) Gazz.chim.ital., 38, I, 427; II,
507-
Muthmann and Kuntze.
(1894) Z.Kryst.Min., 23, 368.
Muthmann and Rolig.
(1898) Z.anorg.Chem., 16, 455.
(1898) Ber., 31, 1728.
Mylius, F.
(1901) Ber., 34, 2208.
(1911) Ber. 44, 1315.
(1911) Z.anorg.Chem., 70, 209.
Mylius, F. and Dietz.
(1901) Ber., 34, 2774.
(1905) Z.anorg.Chem., 44, 217.
(1905) Ber., 38, 921.
Mylius, F. and Forster.
(1889) Ber., 22, 1 100.
(1892) Ber., 25, 70.
Mylius, F. and Funk, R.
(1897) Ber., 30, 1718.
(1900) Wiss.Abh.p.t.Reichsanstalt, 3,
(1900) Ber., 33, 3686.
Mylius, F. and von Wrochem, J.
(1900) Wiss.Abh.p.t.Reichsanstalt, 3,
462.
(1900) Ber., 33, 3689.
Nacken, R.
(i907a) Nachr.kgl.Ges.Wissenschaft
(Gottingen), 602.
(i907b)Jahrb.Min.Geol.(Beil.Bd.),24,
i.
(i907c)Zentralbl.Min.Geol.,262,30i.
(1910) Sitzber.kgl.preuss.Akad.Wis.,
1016-26.
Nagornow, N. N.
(1911) Z.physik.Chem., 75, 578.
Nanty, T.
(1911) Compt.rend., 152,606.
Narbutt, J. V.
(1905) Z.physik.Chem., 53, 704-712.
Nasini, R. and Ageno, I.
(1910) Z.physik.Chem., 69, 482.
(1911) Gazz.chim.ital., 41, I, 131.
Naumann, Alex.
(1904) Ber., 37, 3600, 4328.
(1909) Ber., 42, 3789.
(1910) Ber., 43, 313.
(1914) Ber., 47, 1370.
Naumann, Alex, and Rucker, A.
(1905) Ber., 38, 2293.
Naumann, Alex, and Schier, A.
(1914) Ber., 47, 249.
Neave, G. B.
(1912) Analyst., 37, 399.
Nernst, W.
(1889) Z.physik.Chem., 4, 379.
(1891) Z.physik.Chem., 8, no.
Newth.
(1900) J.Chem.Soc.(Lond.), 77, 776.
Nicol, W. W. J.
(1891) Phil.Mag.(Lond.), [5], 31, 369,
386.
Nicolardot.
(1916) Compt.rend., 163, 355-7.
Nichols, J. B.
(1918) J.Am.Chem.Soc., 40, 402.
von Niementowski, S. and von Rosz-
kowski, T.
(1897) Z.physik.Chem., 22, 146.
Noelting, F.
(1910) Ann.chim.phys., [8], 19, 486.
Nordenskjold and Lindstrom.
(1869) Pogg.Ann., 136, 314.
Noss, F.
(1912) Dissertation, Graz.
(1912) Landolt and Bornstein " Tab-
ellen," 4th Ed., p. 467.
Noyes, A. A.
(1890) Z.physik.Chem., 6, 248.
(1892) Z.physik.Chem., 9, 606, 623.
Noyes, A. A. and Abbott, C. G.
(1895) Z.physik.Chem., 16, 130.
Noyes, A. A. and Boggs, C. R.
(1911) J.Am.Chem.Soc., 33, 1650.
Noyes, A. A. and Chapin, E. S.
(1898) Z.physik.Chem., 27, 443.
(1899) J.Am.Chem.Soc., 21, 513.
Noyes, A. A. and Clement.
(1894) Z.physik.Chem., 13, 413.
Noyes, A. A. and Farrel, F. S.
(1911) J.Am.Chem.Soc., 33, 1654.
Noyes, A. A. and Hall, F. W.
(1917) J.Am.Chem.Soc., 39, 2529.
Noyes, A. A. and Kohr, D. A.
(1902) J.Am.Chem.Soc., 24, 1144.
(1902-03) Z.physik.Chem., 42, 336-
42.
Noyes, A. A. and Sammet, G. V.
(1903) Z.physik.Chem., 43, 526.
808
AUTHOR INDEX
Noyes, A. A. and Schwartz, D.
(1898) Z.physik.Chem., 27, 279-284.
(1898) J.Am.Chem.Soc., 20, 744.
Noyes, A. A. and Seidenslicker.
(1898) Z.physik.Chem., 27, 359.
Noyes, A. A. and Stewart, M. A.
(1911) J.Am.Chem.Soc., 33, 1658.
Noyes, A. A. and Whitcomb, W. H.
(1905) J.Am.Chem.Soc., 27, 756.
Odaira, I.
(1915) M em. Coll. Sci.( Kyoto), i, 324,
330.
Oddo, B.
(1913) Gazz.chim.ital., 43, II, 275.
Okada, K.
(i9i4)Mem.Coll.Sci.(Kyoto), i, 95-
103.
Olie, Jr., J.
(1906) Z.anorg.Chem., 51, 29-70.
(1907) Z.anorg.Chem., 53, 273-80.
Olivari, F.
(1908) Atti accad.Lincei, [5], 17, II,
512, 584, 717.
(1909) Atti accad.Lincei, [5], 18, II,
96.
(1911) Atti accad.Lincei, [5], 20, I,
470-4.
(1912) Atti accad.Lincei, [5], 21, I,
718.
Ordway.
(1865) Am.Jour.Sci., [2], 40, 173.
Orloff.
(1902) J.Russ.Phys.Chem.Soc., 37,
949-
Orton, K. J. P. and King, H.
(1911) J.Chem.Soc.(Lond.), 99, 1192.
Osaka, Y.
(1903-8) Mem.Coll.Sci.Eng. (Kyoto),
i. 93, 265, 290.
(1909) 7th Int.Cong.Appl.Chem.,
4 A, 308.
(1910) Mem.Coll.Sci.Eng. (Kyoto),
2,21-35.
(1910) Nature (London), 84, 248.
(1910-1 i)Mem. Coll. Sci.Eng. (Kyoto),
3, 58.
(1911) J.Tok.Chem.Soc., 32, 870.
Osaka, Y. and Abe, R.
(1911) Mem.Coll.Sci.Eng. (Kyoto), 3,
51-4-
(1911) J.Tok.Chem.Soc., 32, 446.
Osborne, T. and Harris, I. F.
(1905) Am.Jour.Physiol., 14, 151-
171.
Osipoff and Popoff.
(1903) J.Russ.Phys.Chem.Soc., 35,
637.
Ossendowski, A. M.
(1907) Pharm.J.(Lond.), 79, 575.
U907) J.pharm.chim., [6], 26, 162.
Ost.
(1878) J.prakt.Chem., [2], 17, 232.
Oswald, M.
(1914) Ann.chim., i, 57-79.
(1912) Compt.rend., 155, 1504.
(1912) 8th Int.Cong.Appl.Chem., 2,
205.
Oudemans, A. C. Jr.
(1872) Z.anal.Chem., n, 287.
Padoa, M.
(1904) Atti accad.Lincei, [5], 13, I,
723; II, 31.
Padoa, M. and Rotondi, G.
(1912) Atti accad.Lincei, [5], 21, II,
626.
Padoa, M. and Tibaldi.
(1903) Atti accad.Lincei, [5], 12, II,
1 60.
de Paepe, Desire.
(1911) Bull.soc.chim.Belg., 25, 174.
Pajetta, R.
(1906) Gazz.chim.ital., 36, II, 67, 155,
300.
(1907) Pharm.Jour.(Lond.), 79, 315.
Palazzo and Batelli.
(1883) Atti accad.sci.Torino, 19, 514.
Panfiloff.
(1893) J.Russ.Phys.Chem.Soc., 25,
162.
(1893) Chem.Centralbl., II, 910.
(i893a) J.Russ.Phys.Chem.Soc., 25,
262.
(1894) Z.anorg.Chem., 5, 490.
Parker, E. G.
(1914) J.Phys.Chem., 18, 653.
Parmentier.
• (1887) Compt.rend., 104, 686.
(1892) Compt.rend., 114, 1002.
Parravano, N.
(1909) Gazz.chfm.ital., 39, II, 58.
Parravano, N. and Calcagni, G.
(1908) Atti accad.Lincei, [5], 17, I,
731-8.
(1910) Z.anorg.Chem., 65, i.
Parravano, N. and de Cesaris, P.
(1912) Att accad.Lincei, [5], 21, I,
535-
(i9i2a) Atti accad.Lincei, [5], 21, I,
800.
(i9i2b) Gazz.chim.ital., 42, II, i-
191.
Parravano, N. and Fornaini, M.
(1907) Gazz.chim.ital., 37, II, 521.
(1907) Atti accad.Lincei, [5], 16, II,
465-
Parravano, N. and Mieli, A.
(1908) Atti accad.Lincei, [5], 17, II,
33-4-
(1908) Gazz.chim.ital., 38, II, 536.
Parsons, Chas. L. and Corliss, H. P.
(1910) J.Am.Chem.Soc., 32, 1367.
Parsons, C. L. and Corson, H. P.
(1910) J.Am.Chem.Soc., 32, 1383.
Parsons, C. L. and Perkins, C. L.
(1910) J.Am.Chem.Soc., 32, 1387.
809
AUTHOR INDEX
Parsons, C. L. and Whittemore, C. F.
(1911) J.Am.Chem.Soc., 33, 1933.
Partheil and Ferie.
(1903) Archiv.Pharm., 241, 554.
Partheil and Hubher.
(1903) Archiv.Pharm., 241, 413.
Partington, J. R.
(1911) J.Chem.Soc.(Lond.), 99, 315.
Pascal, P.
(1909) Ann.chim.phys., [8], 16, 374.
(1912) Bull.soc.chim., [4], n, 323,
596, 1033.
(1913) Bull.soc.chim., [4], 13, 746.
(1914) Bull.soc.chim., [4], 15, 454.
Pascal, P. and Normand, L.
(1913) Bull.soc.chim., [4], 13, 154-
202, 879.
Paterno, E. and Ampola, G.
(1897) Gazz.chim.ital., 27, I, 481-
536.
Paterno, E. and Mieli, A.
(1907) Atti accad.Lincei, [5], 16, II,
153-
(1907) Gazz.chim.ital., 37, II, 330.
Paterno, E. and Salimei, G.
(1913) Gazz.chim.ital., 43, II, 245.
Patrick and Aubert.
(1874) Trans. Kansas Acad.Sci., 19.
Patten, H. E. and Mott, W. R.
(1904) J.Phys.Chem., 8, 153.
Patterson, A. M.
(1906) J.Am.Chem.Soc., 28, 1734.
Paul, T.
(1894) Z.physik.Chem., 14, in.
(1896) Z.physik.Chem., 25, 95,
(1901) Arch.Pharm., 239, 64.
(1915) Z.Elektrochem., 21, 543.
(1917) Z.Elektrochem., 23, 65-86.
Paul, Th., Ohlmiiller, W., Heise, R.
and Auerbach, Fr.
(1906) Arb.Kaiserl.Gesundheitsamt.,
23, 333-388.
Pawlewski, Br.
(1893) Anzeiger Akad.Wiss.Krakau,
p. 379.
(1898) Ber., 30, 2806.
(1899) Ber., 32, 1040.
(1900) Ber., 33, 1223.
Pawlewski, Br. and Filemonowicz.
(1888) Ber., 21, 2973.
Payen.
(1852) Compt.rend., 34, 356.
Pearce, J. N. and Fry, E. J.
(1914) J.Phys.Chem., 18, 667.
Pearce, J. N. and Moore, T. E.
(1913) Am.Chem.Jour., 50, 218.
Peddle, C. J. and Turner, W. E. S.
(1913) J.Chem.Soc.(Lond.), 103,
1205.
Pelabon.
(1897) Compt.rend., 124, 35.
(1904) J.chim.phys., 2, 320.
(1907) Compt.rend., 145, 118.
Pelabon.
(1908) Compt.rend., 146, 975.
(1909) Ann.chim.phys. [8], 17, 526-
66.
(1913) Compt.rend., 156, 705-7.
Pelet-Jolivet.
(1909) Revue gen. mat. col., p. 249.
Pellini, G.
(1906) Gazz.chim.ital., 36, II, 461.
(i9o6a) Atti accad.Lincei, [5], 15, I,
629.
(1909) Atti accad.Lincei, [5], 18, I,
703; II, 21, 280.
(1910) Atti accad.Lincei, [5], 19, I,
331-
Pellini, G. and Amadori, M.
(1912) Atti accad.Lincei, [5], 21, I,
294.
Pellini, G. and Coppola, A.
(1913) Atti accad.Lincei, [5], 23, I,
147.
Pellini, G. and Pedrina, S.
(1908) Atti accad.Lincei, [5], 17, II
78.
Pellini, G. and Vio, G.
(1906) Atti accad.Lincei, [5], 15, II,
46-53.
Pelouze.
(1869) Compt.rend., 68, 1179; 69, 56.
Penny.
(1855) Phil.Mag., [4], 10, 401.
Perman, E. P.
(1901) J. Chem.Soc.(Lond.), 79, 718.
(1902) J.Chem.Soc.(Lond.), 81, 480.
(1903) J.Chem.Soc.(Lond.)( 83, 1168.
Pettersson, O. and Sonden, K.
(1889) Ber., 22, 1439.
Pfannl, M.
(1911) Monatsh.Chem., 32, 250.
Pfaundler and Schnegg.
(1875) Sitzber.k.Akad.Wis.(Wien).,
?i, II, 351-
Pfeiffer, H.
(1892) Z.physik.Chem., 9, 469.
Pfeiffer, Geo. J.
(1897) Z.anorg.Chem., 15, 194-203.
Pfeiffer, P. and Modelski, J. v.
(1912) Z.physiol.Chem., 81, 331-3.
Pfeiffer, P. and Wurgler.
(1915) Ber., 48, 1939.
(1916) Z.physiol.Chem., 97, 128-47.
Phelps, I. K. and Palmer, H. E.
(1917) J.Am.Chem.Soc., 39, 140.
Philip, James C.
(1903) T.Chem.Soc.(Lond-), 83, 814.
(1905) j.Chem.Soc.(Lond.), 87, 992.
-(1913) J.Chem.Soc.(Lond.), 103, 284.
Philip, J. C. and Bramley, A.
(1915) J.Chem.Soc.(Lond.), 107,
377-387, 1832-
Philip, J. C. and Garner, F. B.
(1909) J.Chem.Soc.(Lond.), 95,
1466-73.
8lO
AUTHOR INDEX
Philip, J. C. and Smith, S. H.
(1905) J.Chem.Soc.(Lond.), 87,
I735-I75L
Pickering, S. U.
(1890) J.Chem.Soc.(Lond.), 57, 331-
(1890-91) Proc.Roy.Soc.(Lond.), 49,
25-
(1893) J.Chem.Soc.(Lond.), 63, 141,
463, 909, 998.
(i893a) Ben, 26, 2307.
(1895) J.Chem.Soc.(Lond.), 67, 669.
(1912) Landolt and Bornstein,
" Tabellen," 4th Ed., p. 471.
(1915) J.Chem.Soc.(Lond.), 107,
942-54.
Pictet, Raoul.
(1894) Compt.rend., 119, 642.
Pictet, R. and Altschul, M.
(1895) Z.physik.Chem., 16, 78.
(1894) Compt.rend., 119, 678-82.
Pierre.
(1847) J.pharm.chim., [3], 12, 237.
Pina de Rubies, S.
(1913) Anales soc.espan.fis.quin., n,
422-35-
(1914) Anales soc.espan.fis.quin., 12,
343-9;
(1914) Archiv.sci.physique,naturelle
(Madrid), [4], 38, 414-22.
(1915) Chem.Zentralbl., I, 521.
Pinnow, J.
(1911) Z.anal.Chem., 50, 162.
(1915) Z.anal.Chem., 54, 321-345-
Plato,
(1907) Z.physik.Chem., 58, 350.
Pleissner, M.
(1907) Arb.Kais.Gesundheitsamt, 26,
384-443.
Plotnikow, W. A.
(1911) Ann. inst.Polytech. Kiev., n,
310.
(1915) J.Russ.Phys.Chem.Soc., 47,
1062-4.
Poggiale.
(1843) Ann.chim.phys., [3], 8, 467.
Pohl.
(1852) J.prakt.Chem., 56, 216.
(1860) Sitzber.k.Akad.Wiss.(Wien),
41, 627.
Pollacci.
(1896) L'Orosi, 19, 217.
Pollitzer, F.
(1909) Z.anorg.Chem., 64, 121-48.
Poma, G.
(1909) Atti accad.Lincei, [5], 18, I,
133-8.
(1910) Gazz.chim.ital., 40, I, 197.
Poma, G. and Gabbi, G.
(1912) Gazz.chim.ital., 42, II, 8.
(1911) Atti accad.Lincei, [5], 20, I,
464-70.
Porlezza, C.
(1914) Atti accad.Lincei, [5], 23, II,
* * 5°9' 597'
Power, F. B.
(1882) Am.Jour.Pharm., 54, 97-99.
Power, F. B. and Tutin.
(1905) J.Chem.Soc.(Lond-), 87, 24.
Pratolongo, U.
(1913) Atti accad.Lincei, [5], 22, I,
388.
(1914) Atti accad.Lincei, [5], 23, 1, 46.
Pratt, L. A. and James, C.
(1911) J.Am.Chem.Soc., 33, 488.
Precht, H. and Wittgen, B.
(1881) Ber., 14, 1667.
(1882) Ber., 15, 1666.
Presse, C. H.
(1874) Ber., 7, 599.
Prins, Ada.
(1909) Z.physik.Chem., 67, 689-722.
Prunier.
(1879) J.pharm.chim., [4], 29, 136.
Puckner, W. A. and Hilpert, W. S.
(1909) J.Am.Med.Assoc., 52, 311.
Puckner, W. A. and Warren, L. E.
(1910) Proc.Am.Pharm.Assoc., 58,
1007.
(1910) Lab. Reports Am.Med.Assoc.,
3> 123.
Puschin, N. A. and Baskow, A.
(1913) Z.anorg.Chem., 81, 347-63.
Puschin, N. A. and Glagoleva, A. A.
(1914) Ann.Inst.Electrotechnique
(Petrograd), n, 284.
(1915) J.Russ.Phys.Chem.Soc., 47,
100-13.
Pushin, N. A. and Grebenschikov, I. V.
(1913) J.Russ.Phys.Chem.Soc., 45,
741-5-
Pushin, N. and Kriger, J.
(1913) Ann.Inst.Electrotechnique
(Petrograd), 9, 235.
(1914) J.Russ.Phys.Chem.Soc., 46,
559-
Pushin, N. A. and Mazarovich, G. M.
(1914) J.Russ.Phys.Chem.Soc., 46,
1366-72.
(1914) Ann.Inst.Electrotechnique
(Petrograd), 10, 205.
Quercigh, E.
(1912) Atti accad.(Lincei), [5], 21, I,
417, 786.
(1914) Atti accad.(Lincei), [5], 23, I,
449, 825.
Rabe, W. O.
(1901) Z.physik.Chem., 38, 175-184.
(1902) Z.anorg.Chem., 31, 156.
Rack, G.
(1914) Centr.Min.Geol., 326-8.
Radan.
(1889) Liebig's Ann., 251, 129.
811
AUTHOR INDEX
Raffo, M. and Rossi, G.
(1915) Gazz.chim.ital., 45, I, 45-
Rammelsberg.
(1838) Pogg.Ann., 43, 665; 44, 575-
(1841) Pogg.Ann., 52, 81, 96.
(1892) J.prakt.Chem., [2], 45, 153.
Ramstedt, Eva.
(1911) Radium, 8, 253^6.
Rankin, G. A. and Merwin, H. E.
(1916) J.Am.Chem.Soc., 38, 568.
Rankin, G. A. and Wright.
(1915) Am.Jour.Sci., [4], 39, i~79.
Raoult.
(1874) Ann.chim., [5], i, 262.
Raupenstrauch, G. A.
(1885) Monatsh.Chem., 6, 585.
Rebiere, G.
(1915) Bull.soc.chim., [4], 17, 268,
Regnault and Wiilejean.
(1887) Chem.Centralbl., 18, 252.
Reich.
(1891) Monatsh.Chem., 12, 464.
Reichel, H.
(1909) Biochem.Ztschr., 22, 156.
Reicher, L. T. and van Deventer, C. M.
(1890) Z.physik.Chem., 5, 560.
Reid.
(1887-88) Proc.Roy.Soc.(Edin.), 15,
151-
Reid, H. S. and Mclntosh, D.
(1916) J.Am.Chem.Soc., 38, 615-25.
Reinders, W.
(1900) Z.physik.Chem., 32, 494, 514.
(1906) Z.physik.Chem., 54, 609.
(1914) Proc.k.Akad.Wet.(Amst.), 16,
1065.
(1915) Z.anorg.Chem., 93, 202.
Reinders, W. and de Lange, S.
(1912-13) Z.anorg.Chem., 79, 230.
(1912) Proc.k.Akad.Wet.(Amst.), 15,
474-
Reinders, W. and Lely, Jr. D.
(1912) Proc.k.Akad.Wet.(Amst.), 15,
486.
Reinitzer, D.
(1913) Z.angew.Chem., 26, 456.
Reissig.
(1863) Liebig's Ann., 127, 33.
Retgers, J. W.
(1893) Z.anorg.Chem., 3, 253, 344.
(1893) Rec.trav.chim., 12, 229.
Rex.
(1906) Z.physik.Chem., 55, 355.
Reychler, A.
(1910) J.chim.phys., 8, 618.
Reynolds, J. E. and Werner, E. A.
(1903) J.Chem.Soc.(Lond.}, 83, 5.
Richards, T. W.
(1897) Z.anorg.Chem., 3, 455.
Richards, T. W. and Archibald, E. H.
(1901-02) Proc.Am.Acad., 37, 345.
(1902) Z.physik.Chem., 40, 385-98.
Richards, T. W. and Churchill.
(1899) Z.physik.Chem., 28, 314.
Richards, T. W. and Faber, H. B.
(1899) Am.Chem.Jour., 21, 167-172.
Richards, T. W. and Kelley.
(1911) J.Am.Chem.Soc., 33, 847.
Richards, T. W., McCaffrey and Bisbee.
(1901) Z.anorg.Chem., 28, 85.
Richards, T. W. and Meldrum, W. B.
(1917) J.Am.Chem.Soc., 39, 1821-2.
Riedel.
(1906) Z.physik.Chem., 56, 243.
Riesenfeld, E. H.
(1902) Z.physik.Chem., 41, 346.
(1903) Z.physik.Chem., 45, 461.
Riley, W. A.
(1911) Jour.Inst. Brewing, 17, 124.
(1911) " Tables annuelles," 2, 428.
Rimbach, E.
(1897) Ber., 30, 3079.
(1902) Ber., 35, 1300.
(1904) Ber., 37, 463.
(1905) Ber., 38, 1553-7, 1570.
Rimbach, E. and Korten, F.
(1907) Z.anorg.Chem., 52, 407.
Rimbach, E. and Schubert, A.
(1909) Z.physik.Chem., 67, 183-200.
Rindell, A.
(1910) Z.physik.Chem., 70, 452-8.
Ringer, W. E.
(1902) Z.anorg.Chem., 32, 212.
(1902) Rec.trav.chim., 21, 374.
Ritzel, A.
(1911) Z.Kryst.Min., 49, 152.
Robertson, B.
(1908) J.Biol.Chem., 5, 147-54.
Robertson, P. W.
(1907) Chem.News, 95, 253.
Robinet.
(1864) Compt.rend., 58, 608.
Robinson, F. W.
(1909) J.Chem.Soc.(Lond.), 95,
1353-9-
Robinson, W. O. and Waggaman, W.H.
(1909) J.Phys.Chem., 13, 673-8.
Rodt, V.
(1916) Mitt.k. Materials prufungs-
amt, 33, 426-33.
(1916) Chem.Zentr., I, 1270.
Rodwell.
(1862) J.Chem.Soc.(Lond.), 15, 59.
Roelofsen.
(1894) Am.Chem.Jour., 16, 466.
Rogier and Fiore.
(1913) Bull.sci.Pharmacologique, 20,
7, 72.
Rohland, P.
(1897) Z.anorg.Chem., 15, 412.
(1898) Z.anorg.Chem., 18, 328.
Roloff, M.
(1894) Z.physik.Chem., 13, 341.
(1895) Z.physik.Chem., 17, 325-56.
(1895) Z.physik.Chem., 18, 572-84.
812
AUTHOR INDEX
Roozeboom, H. W. B.
(1884) Rec.trav.chim., 3, 29-87.
(1885) Rec.trav.chim., 4, 69.
(1887) Rec.trav.chim., 6, 342.
(1888) Z.physik.Chem., 2, 459, 518.
(1889) Rec.trav.chim., 8, 1-146.
(1890) Z.physik.Chem., 5, 201.
(1891) Z.physik.Chem., 8, 532.
(1891) Rec.trav.chim., 10, 271.
(1892) Z.physik.Chem., 10, 477.
(1893) Rec.trav.chim., 12, 205.
(1899) Proc.k.Akad.Wet.(Amst.), I,
466.
Roscoe.
(1866) J.Chem.Soc.(Lond.), 19, 504.
Roscoe and Dittmar.
(1859) Liebig's Annalen, 112-234.
Rosenbladt.
(1886) Ber., 19, 2531.
Rosenheim, A. and Bertheim, A.
(1903) Z.anorg.Chem., 34, 430.
Rosenheim, A. and Davidsohn, I.
(1903) Z.anorg.Chem., 37, 315.
Rosenheim, A. and Griinbaum.
(1909) Z.anorg.Chem., 61, 187.
Rosenheim, A. and Pritze, M.
(1908) Ber., 41, 2708.
(1909) Z.anorg.Chem., 63, 275-81.
Rosenheim, A., Stadler and Jakobsohn.
(1906) Ber., 39, 2841.
Rosenheim, A. and Weinheber, M.
(1910-11) Z.anorg.Chem., 69, 263.
Roshdestwensky, A. and Lewis W. C.
McC.
(1911) J.Chem.Soc.(Lond.), 99, 2144.
(1912) J.Chem.Soc.(Lond.), 101,
2098.
van Rossem, C:
(1908) Z.physik.Chem., 62, 681-712.
Rossler.
(1873) J.prakt.Chem., [2], 7, 14.
Roth.
(1897) Z.physik.Chem., 24, 123.
Rothmund, V.
(1898) Z.physik.Chem., 26, 459, 475.
(1900) Z.physik.Chem., 33, 406.
(1908) Z.Elektrochem., 14, 532.
(1910) Z.physik.Chem., 69, 523-546.
(1912) Nernst. Festschrift, 391-4.
(1912) Chem.Zentr., II, 1261.
Rothmund, V. and Wilsmore, N. T. M.
(1898) Z.physik.Chem., 26, 475.
(1902) Z.physik.Chem., 40, 623.
Rotinjanz, L. and Rotarski, T.
(1906) J.Russ.Phys.Chem.Soc., 38,
782.
Rozsa, M.
(1911) Z. Elektrochem, 17, 935.
Rubenbauer.
(1902) Z.anorg.Chem., 30, 334.
Rudorff.
(1862) Pogg.Ann., 116, 63.
(1869) Ber., 2, 70.
Rudorff.
(1872) Pogg.Ann., 145, 608.
(1873) Ber., 6, 482.
(1885) Ber., 18, 1160.
Ruer.
(1906) Z.anorg.Chem., 49, 365.
Ruff, Otto.
(1909) Ber., 42, 4029.
Ruff, Otto and Fischer, G.
(1903) Ber., 36, 418-428.
Ruff, O. and Hecht, L.
(1911) Z.anorg.Chem., 70, 61.
Ruff, Otto and Geisel, E.
(1906) Ber., 39, 838.
Ruff, Otto and Plato, W.
(1903) Ber., 36, 2358-2365.
Ruff, O. and Schiller, E.
(1911) Z.anorg.Chem., 72, 341.
Ruff, O. and Winterfeld.
(1903) Ber., 36, 2437.
Rupert, F. F.
(1909) J.Am.Chem.Soc., 31, 866.
(1910) J.Am.Chem.Soc., 32, 748.
Rutten and van Bemmelen.
(1902) Z.anorg.Chem., 30, 386.
Ryd, S.
(1917) Z.Elektrochem., 23, 19-23.
S.
(1905) Apoth.Ztg., 20, 1031.
Sackur, O.
(1911-2) Z.physik.Chem., 78, 553-
568.
(1913) Z.physik.Chem., 83, 297-314.
Sackur, O. and Fritzmann, E.
(1909) Z.Elektrochem., 15, 842-6.
Sackur, O. and Taegener, W.
(1912) Z.Elektrochem., 18, 722.
Sahmen, R.
(1905-06) Z.physik.Chem., 54, m-
120.
Sakabe, S.
(1914) Mem.Coll.Sci. (Kyoto), i, 57-
61.
Salkowski, H.
(1883) Ber., 18, 321.
(1901) Ber., 34, 1947.
Salkower, B.
(1916) Am.J.Pharm., 88, 484.
Salzer.
(1886) Liebig's Ann., 232, 114.
Sammet, V.
(1905) Z.physik.Chem., 53, 644-48.
Sander, W.
(1911-12) Z.physik.Chem., 78, 513-
549-
Sandonmm, C.
(1911) Atti accad.Lincei, [5], 20, I,
• 173, 253.
(1911) Gazz.chim.ital., 41, II, 146.
(1911) Atti accad.Lincei, [5], 20, II,
62, 497, 572, 588, 646.
(191 la) Atti accad.Lincei, [5], 20, I,
457, 76o.
813
AUTHOR INDEX
Sandonnini, C.
(1912) Atti accad.Lincei, [5], 21, I,
208-13, 479.
(i9i2a) Atti accad.Lincei, [5], 21, II,
197, 524» 635.
(i9i2b) Atti Ist.Ven., 71, 553.
(1913) Atti accad.Lincei, [5], 22, I,
630; II, 21.
(1914) Atti accad.Lincei, [5], 23, I,
962.
(1914) Gazz.chim.ital., 44, 1, 296, 382
Sandonnini, C. and Aureggi, P. C.
(1912) Atti accad.Lincei, [5], 21, I,
493-
Sandonnini, C. and Scarpa, G.
(191 la) Atti accad.Lincei, [5], 20, II,
62.
(191 ib) Atti accad.Lincei, [5], 20, II,
497-
(1912) Atti accad.Lincei, [5], 21, II,
77-84.
(1913) Atti accad.Lincei, [5], 22, II,
21, 163, 518.
Sandquist, H.
(1911) Liebig's Ann., 379, 85.
(1912) Liebig's Ann., 392, 76.
Ark.Kem.Min.Geol., 4, 8-8 1.
Saposchinikow, Gelvich et al.
(1903) J.Russ.Phys.Chem.Soc., 35,
(1904) Z.physik.Chem., 49, 688-96.
Savorro, Eglie.
(1914) Atti accad.sci. (Torino), 48,
948-59.
(1914) Chem.Abs., 8, 340.
Sborgi, U.
(1913) Atti accad.Lincei, [5], 22, I,
91, 636, 716, 798.
(1915) Atti accad.Lincei, [5], 24, I,
1225.
Sborgi, U. and Mecacci, F.
(1915) Atti accad.Lincei, [5], 24, I,
443—8.
(1916) Atti accad.Lincei, [5], 25, II,
327, 386, 455.
Scaffidi, V.
(1907) Z.physik.Chem., 52, 42.
Scarpa, G.
(1912) Atti accad.Lincei, [5], 21, II,
720.
(1915) Atti accad.Lincei, [5], 24, I,
741, 955; II, 476.
Scarpa, O.
(1904) J.chim.phys., 2, 449.
Schachner, Paul.
(1910) Biochem.Centralbl., 9, 610.
Schaefer, G. L.
1910) Am.Jour.Pharm., 82, 175.
1910) Pharm.Jour.(Lond.), 84, 757.
1912) Am.Jour.Pharm., 84, 389.
(1913) Am.Jour.Pharm., 85, 441.
Schafer, H.
(1905) Z.anorg.Chem., 45, 310.
Schaefer, W.
(1914) Neues Jahrb.Min.Geol., I, 15-
24.
von Scheele, C.
(1899) Ber., 32, 415.
Scheffer, F. E. C.
(1911) Proc.k.Akad.Wet.(Amst.), 13,
829; 14, 195.
(1912) Z.physik.Chem., 76, 161.
(i9i2a) Proc.k.Akad.Wet.(Amst.),
15, 38o.
Scheibler, C.
(1872) Ber., 5, 343.
(1883) J.pharm.chim., [5], 8, 540.
(1891) Ber., 24, 434.
Schenck, R. and Rassbach, W.
(1908) Ber., 41, 2917.
Scheuble, R.
(1907) Liebig's Ann., 351, 473-80.
Scheuer, Otto.
(1910) Z.physik.Chem., 72, 525-35.
Schiavor, G.
(1902) Gazz.chim.ital., 32, II, 532.
Schick, K.
(1903) Z.physik.Chem., 42, 163.
Schierholz.
(1890) Sitzber.k.Akad.Wiss.(Wien.),
101, 2&, 4.
Schiff.
(1859) Liebig's Ann., 109, 326.
(1860) Liebig's Ann., 113, 350.
(1861) Liebig's Ann., 118, 365.
Schiff and Monsacchi.
(1896) Z.physik.Chem., 21, 277.
Schindelmeiser.
(1901) Chem.Ztg., 25, 129.
Schlamp, A.
(1894) Z.physik.Chem., 14, 272.
Schloesing.
(1871) Compt.rend., 73, 1273.
(1872) Compt.rend., 74, 1552; 75, 70.
Schlossberg, J.
(1900) Ber., 33, 1082.
Schmidlin, J. and Lang, R.
(1910) Ber., 43, 2813.
(1912) Ber., 45, 905.
Scholl, R. and Steinkopf.
(1906) Ber., 39, 4393.
Scholtz, M.
(1901) Ber., 34, 1623.
(1912) Arch.Pharm., 250, 418.
Scheme.
(1873) Ber., 6, 1224.
Schonfeld.
(1885) Liebig's Ann., 95, 5.
Schoorl, N.
(1903) Rec.trav.chim., 22, 40.
Schrefeld.
(1894) Z.Ver.Zuckerind, 44, 971.
Schreinemakers, F. A. H.
(1892) Z.physik.Chem., 9, 65, 71.
(1897) Z.physik.Chem., 23, 417-41.
(1898) Z.physik.Chem., 25, 543-67.
814
AUTHOR INDEX
Schreinemakers, F. A. H.
(1898) Z.physik.Chem., 26, 237-54.
(18980) Z.physik.Chem., 27, 95-122.
(1899) Z.physik.Chem., 29, 577.
(1900) Proc.k.Akad.Wet.(Amst.), 2,
i.
(1900) Z.physik.Chem., 33, 79.
(1903) Z.anorg.Chem., 37, 207.
(1906) Z.physik.Chem., 55, 89.
(1907) Z.physik.Chem., 59, 641.
(1908-09) Z.physik.Chem., 65, 555,
575-
(1908) Chem.Weekblad., 5, 847.
(1909) Z.physik.Chem., 66, 687-98.
(1909) Chem.Weekblad., 6, 131, 140.
(1909-10) Z.physik.Chem., 68, 83-
103.
(1910) Arch.neer.sc.ex.nat., [2], 15,
81, 117.
1910) Z.physik.Chem., 69, 557~68.
ioa) Z.physik.Chem., 71, 109-16.
I9iob) Chem.Weekblad., 7, 333.
1911) Proc.k.Akad.Wet.(AmstJ, 13,
1163.
Schreinemakers, F. A. H. and de Baat,
W. C.
(1908) Chem.Weekbl., 5, 465-72.
(1908-9) Z.physik.Chem., 65, 586.
(1909) Z.physik.Chem., 67, 551-60.
(1910) Chem.Weekblad., 7, 259.
(igioa) Arch.neer.sc.ex.nat., [2], 15,
4-15-
(1914) Proc.k.Akad.Wet.(Amst.), 17,
533, 78i.
(1915) Proc.k.Akad.Wet.(Amst.), 17,
mi.
(1915) Verslag.k.Akad.Wet.(Amst.),
23, 1097; May.
(1917) Chem.Weekblad., 14, 141,
203, 244.
(1917) Chem. Weekblad., 14, 262-7,
288.
Schreinemakers, F.A.H. and Cocheret,
D. H.
(1905) Chem.Weekblad., 2, 771-778.
Schreinemakers, F. A. H. and Cocheret,
D. H., Filippo, H. and de
Waal, A. J. C.
(1901) Z.physik.Chem., 59, 645.
Schreinemakers, F. A. H. and Deuss,
J. J. B.
(1912) Z.physik.Chem., 79, 554.
Schreinemakers, F. A. H. and Van
Dorp, W. A. Jr.
(1906) Chem.Weekblad., 3, 557-561.
(1907) Z.physik.Chem., 59, 641-69.
Schreinemakers, F. A. H. and Figee, T.
(1911) Chem.Weekblad., 8, 683-8.
Schreinemakers, F. A. H. and Filippo,
A. Jr.
(1906) Chem.Weekblad., 3, 157-165.
(1906) Chem.Zentralbl., 77, I, 1321.
Schreinemakers, F. A. H. and Hoenen,
P. H. J.
(1909) Chem.Weekblad., 6, 51.
Schreinemakers, F. A. H. and Van der
Horn van den Bos, J.
L.M.
(1912) Z.physik.Chem., 79, 551.
Schreinemakers, F. A. H. and Jacobs,
W.
(1910) Chem.Weekblad., 7, 215.
Schreinemakers, F. A. H. and Massink,
A.
(1910) Chem.Weekblad., 7, 214.
Schreinemakers, F. A. H. and Mei-
jeringh, D. J.
(1908) Chem.Weekblad., 5, 811.
Schreinemakers, F. A. H. and Van
Provije, D. J.
(1913) Proc.k.Akad.Wet., 15, 1326.
Schreinemakers, F. A. H. and Thonus,
J. C.
(1912) Proc.k.Akad.Wet.(Amst.), 15,
472.
Schroder.
(1893) Z.physik.Chem., u, 449.
Schroeder, J.
(1905) Z.anorg.Chem., 44, 6.
(1908) J.prakt.Chem., [2], 77, 267-8.
Schiikarew, A.
(1901) Z.physik.Chem., 38, 543.
Schukow.
(1900) Z.Ver.Zuckerind, 50, 313.
Schuler.
(1879) Sitzb.k.Akad.Wis. (Berlin), 79,
302.
Schultz.
(1860) Zeit.Chem., [2], 5, 531.
(1861) Pogg.Ann., 113, 137.
Schulze.
(1881) J.prakt.Chem., [2], 24, 168.
Schweissinger.
(1884-85) Pharm.Ztg.
Schweitzer.
(1890) Z.anal.Chem., 29, 414.
Schwicker.
(1889) Ber., 22, 1731.
Sedlitzky.
(1887) Monatsh.Chem., 8, 563.
Seidell, A.
1902) Am.Chem.Jour., 27, 52.
1907) J.Am.Chem.Soc., 29, 1088-95.
1908) Trans. Am. Electrochem.Soc.,
13, 319-329-
(1909) J.Am.Chem.Soc., 31, 1164.
(1910) Bull.No.67 Hygienic Labora-
tory, U. S. Public Health
Service,
(igioa) Proc.Am.Pharm.Assoc., 58,
1031.
(1912) Am.Chem.Jour., 48, 453-67.
Seidell, A. and Smith, J. G.
(1904) J.Phys.Chem., 8, 493.
815
AUTHOR INDEX
Self, P. A. W. and Greenish, H. G.
(1907) Pharm.Jour.(Lond.), 78, 327.
Seliwanow, Th.
(1914) Z.anorg.Chem., 85, 337.
Sehnal, J.
(1909) Compt.rend., 148, 1394.
Serullas.
( ) Ann.chim.phys., 22, 118.
Sestini.
(1890) Gazz.chim.ital., 20, 313.
Setschenow.
(1892) Ann.chim.phys., [6], 25, 226.
Setterburg.
(1882) Liebig's Annalen, 211, 104.
Seubert and Elten.
(1892) Z.anorg.Chem., 2, 434.
Seyler, C. A.
(1908) Analyst, 33, 454~7-
Seyler, C. A. and Lloyd, P. V.
(1909) J.Chem.Soc.(Lond.), 95>I347~
Shad, H. and Bornemann, K.
(1916) Metall u.Erz., 13, 251-62.
Sharwood, W. J.
(1903) J.Am.Chem.Soc., 25, 576.
Sherrill, M. S.
(1903) Z.physik.Chem., 43, 705-740.
Sherrill, M. S. and Eaton, F. M.
(1907) J.Am.Chem.Soc., 29, 1643.
Sherrill, M. S. and Russ, D. E.
(1907) J.Am.Chem.Soc., 29, 1657-61.
Shiomi, T.
(1908) Mem.Coll.Sci.Eng. (Kyoto), i,
406-13.
Sidgwick, N. V.
(1910) Proc.Chem.Soc.(Lond.), 26,
60-1.
(1911) J.Chem.Soc.(Lond.),99, 1123.
(1915) J.Chem.Soc.(Lond.), 107, 672.
Sidgwick, N. V., Pickford, P. and Wils-
don, B. H.
(1911) J.Chem.Soc.(Lond.),9Q,ii22-
1132.
Sidgwick, N. V., Spurrell, W. J. and
Davies, T. E.
(1915) J.Chem.Soc.(Lond.), 107,
1202-13.
Siebeck.
(1909) Scand.Arch.f.Physiol., 21, 368.
Sieger, W.
( ) Dissertation, Delft, 156.
(1912) "Tables, annuelles," 3, 337.
Sieverts, A. and Co-workers.
(1909) Ber., 42, 338.
(1910) Ber., 43, 893.
(1912) Ber., 45, 221.
Sieverts, A. and Bergner, E.
"- 4s>
(1905) Z.physik.Chem., 51, 577-602.
(1916) J.Am.Chem.Soc., 38, 2632.
Sims.
(1861) Liebig's Ann., 118, 340.
Sinnige, L. R.
(1909) Z.physik.Chem., 67, 432-45.
Sisley, P.
(1902) Bull.soc.chim., [3], 27, 905.
Skirrow, F. W.
(1902) Z.physik.Chem., 41, 144.
Skinner, S.
(1892) J.Chem.Soc.(Lond.), 61, 342.
Skossareswky, M. and Tchitchinadze,
(1916) J.chim.phys., 14, 153-175.
Skrabal, A.
(1917) Monatsh.Chem., 38, 25-9.
Slade, R. E.
(1912) Z.Elecktrochem., 18, i.
Sloan and Mallet.
(1882) Chem.News., 46, 194.
Slothouwer, J. H.
(1914) Rec.trav.chim., 33, 327.
Smirnoff, Wladimer.
(1907) Z.physik.Chem., 58, 373, 667.
Smith.
(1912) Landolt and Bornstein "Tab-
ellen," 4th Ed., p. 481.
Smith and Bradbury.
(1891) Ber., 24, 2930.
Smith, A. and Carson, C. M.
(1908) Z.physik.Chem., 61, 200.
Smith, A. and Eastlack, H. E.
(1916) J.Am.Chem.Soc., 38, 1500,
1265.
Smith, A., Holmes, W. B. and Hall, E.S.
(1905) J.Am.Chem.Soc., 27, 805.
Smith, A. and Menzies, A. W. C.
(1909) J.Am.Chem.Soc., 31, 1183-91.
Smith, C. and Watts, C. H.
(1910) J.Chem.Soc.(Lond.), 97, 568.
Smith, F. Hastings.
(1917) J.Am.Chem.Soc., 39, 1309.
Smith, G. McP. and Ball, T. R.
(1917) J. Am.Chem.Soc., 39, 217.
Smith, Herbert, J.
(1918) J.Am.Chem.Soc., 40, 879-885.
Smith, W. R.
(1909) J.Am.Chem.Soc., 31, 245.
Smits, A.
(1903) Z.Elecktrochem, 9, 663.
Smits, A. and Bokhorst, S. C.
(1915) Z.physik.Chem., 89, 374.
Smits, A. and Kettner, A.
(1912) Proc.k.Akad.Wet.(Amst.), 15,
685.
Smits, A. and de Leeuw, H. L.
(1910) Proc.k.Akad.Wet.(Amst.), 13,
329-
Smits, A. and Maarse, J.
(1911) Proc.k.Akad.Wet.(Amst.), 14,
192.
Smits, A. and de Mooy.
(1910) Verslag.Akad.Wet.(Amst.),
19, 293.
816
AUTHOR INDEX
Smits, A. and Postma, S.
(1914) Proc.k.Akad.Wet.(Amst.), 17,
183-
Smolensky, S.
(1911-12) Z.anorg.Chem., 73, 293.
Sneider.
(1866) Pogg.Ann., 127, 624.
Snell, J. F.
(1898) J.Phys.Chem., 2, 474, 484.
Snyder.
(1878) Ber., n, 936.
Soch, C. A.
(1898) J.Phys.Chem., 2, 43.
Sommer, F.
(1914) Z.anorg.Chem., 86, 85.
Sosman, R. B. and Merwin, H. E.
(1916) J.Wash.Acad.Sci., 6, 532-537-
Souchay and Leussen.
(1856) Liebig's Ann., 99, 33.
Spencer, J. F.
(1912) Z.physik.Chem., 80, 701.
(1913) Z.physik.Chem., 33, 293.
Spencer and LePla.
(1909) Z.anorg.Chem., 65, 14.
Speyers, C. L.
(1902) Am.J.Sci., [4], 14, 294.
Spielrein, C.
(1913) Compt.rend., 157, 46.
Spring and Romanoff.
(1896) Z.anorg.Chem., 13, 34.
Squire, P. W. and Caines, C. M.
(1905) Pharm.Jour.(Lond.), 74, 720,
784.
v. Stackelberg, E. F.
(1896) Z.physik.Chem., 20, 337-58.
van der Stadt, E.
(1902) Z.physik.Chem., 41, 353.
Stanley, H.
(1904) Chem.News, 89, 193.
Stark, G.
(1911) Z.anorg.Chem., 70, 174.
Steger.
(1903) Z.physik.Chem., 43, 595.
Stern, Otto.
(1912-13) Z.physik.Chem., 81, 468.
Staronka, W.
(1910) Anzeiger akad.Wis.Krakau.
Ser.A., 372-98.
(1910) Chem.Zentralbl., 81, 1741.
Stasevich, N.
(1913) J.Russ.Phys.Chem.Soc., 45,
912-30.
Steele and Johnson.
(1904) J.Chem.Soc.(Lond.), 85, 116.
Steiner, P.
( 1 894) Ann.der. Physik. ( Wiederman) ,
52, 275.
Stemwehr.
(1902) Ann.der Physik. (Drude), [4],
9, 1050.
Stepanow, A.
(1907) Z.ges.Schiess.u.Sprengstoffw.,
Stepano, A.
(1910) J.Russ.Phys.Chem.Soc., 42,
489.
(1910) Liebig's Ann., 373, 219.
Stiassny.
(1891) Monatsh.Chem., 12, 601.
Stich, C.
(1903) Pharm.Ztg., 48, 343.
(1903) Pharm.Jour.(Lond.), 70, 700.
Stock, A.
(1904) Ber., 37, 1432.
(1910) Ber., 43, 156, 1227.
Stock, A. and Kuss, E.
(1917) Ber., 50, 159-164-
Stoermer, R. and Heymann, P.
(1913) Ber., 46, 1255.
Stolba.
(1865) J.prakt.Chem., 94, 406.
(1867) J.prakt.Chem., 101, I.
(1872) Z.anal.Chem., n, 199.
(1877) Chem.Centralbl., 418, 578.
(1883) Chem.Centralbl., 293.
(1889) Chem.Techn.Cent., Anz., 7,
Stolle. 459'
(1900) Z.Ver.Zuckerind., 50, 331.
Stoltzenberg, H.
(1912) Ber., 45, 2248.
(1914) Z.physik.Chem., 92, 461-94.
Stortenbecker, W.
(1888) Rec.trav.chim., 7, 152.
(1889) Z.physik.Chem., 3, n.
(1897) Z.physik.Chem., 22, 62.
(1900) Z.physik.Chem., 34, 109.
(1902) Rec.trav.chim., 21, 407.
(1907) Rec.trav.chim., 26, 245.
Straub, Jan.
(1911) Z.physik.Chem., 77, 332.
Stromholm, D.
(1900) Ber., 33, 835.
(1903) Z.physik.Chem., 44, 721-32.
(1908) Z.anorg.Chem., 57, 72-103.
Struve.
1870) Z.anal.Chem., 9, 34.
1899) J.prakt.Chem., [2], 61, 457.
Sudborough, J. J. and Lakhumalani,
J.V.
(1917) J.Chem.Soc.(Lond.), in, 44.
Sudhaus, Kathe.
(1914) Neues Jahrb.Min.Geol.(Beil.
Bd.), 37, 1-50.
Sulc.
(1900) Z.anorg.Chem., 25, 401.
Siiss, J.
(1913) Z.Kryst.Min., 51, 262.
Suyver, J. F.
(1905) Rec.trav.chim., 24, 381, 397.
Swan, Clifford, M.
(1899) " Chemistry Thesis," Mass.
Inst.Technology, (un-
published).
(1911) J.Am.Chem.Soc., 33, 1814.
817
AUTHOR INDEX
Swinne, R.
(1913) Z.physik.Chem., 84, 348.
Szathmary de Szachmar, L. v.
(1910) Z.Farb.Ind., 7, 215.
(1910) Chem.Abs., 4, 1381.
de Szyszkowski, Bohdan.
(1915) Medd.K.Vetenskapsakad,No-
belinst., 3, Nos. 3, 4, 5.
Taber, W. C.
(1906) J.Phys.Chem., 10, 593.
(1906) Bull., 33, Bureau of Soils, U. S.
Dept. Agr.
Tafel, J.
(1901) Ber., 34, 263.
Takenchi, J.
(1915) Mem.Coll.Sci. (Kyoto), 1,249-
55-
Tamm, O.
(1910) Z.physik.Chem., 74, 499.
Tarugi, N.
(1904) Gazz.chim.ital., 34, I, 329.
(1914) Gazz.chim.ital., 44, I, 131.
Tarugi, N. and Checchi, Q.
(1901) Gazz.chim.ital., 31, II, 430,
445-
Taverne, H. J.
(1900) Rec.trav.chim., 19, 109.
Taylor, H. S. and Henderson, W. N.
(1915) J.Am.Chem.Soc., 37, 1692.
Taylor, S. F.
(1897) J.Phys.Chem., i, 301, 468,
720.
Tcherniac, J.
(1916) J.Chem.Soc. (Lond.), 109,1239.
Tetta Polak'van der Goot.
(1913) Z.physik.Chem., 84, 419-50.
Than.
(1862) Liebig's Ann., 123, 187.
Thiel.
(1903) Z.physik.Chem., 43, 656.
Thilo.
(1892) Chem.Ztg., 16, II, 1688.
Thin, R. G. and Gumming, Alex. C.
(1915) J.Chem.Soc.(Lond.), 107,
361-6.
Thomas.
(1896) Compt.rend., 123, 943.
Thomas, J. S. and Rule, A.
(1917) J.Chem.Soc. (Lond.), in,
1063-85.
Thompson, M. de K.
(1910) Met.Chem.Eng., 8, 279, 324.
(1910) Proc.Am.Acad., 45, 431-52.
Thonus, J. C.
(1913) Verslag.k.Akad.Wet.(Amst.),
Thorin, E. G.
(1915) Z.physik.Chem., 89, 687.
Tichomirow, W.
(1907) J.Russ.Phys.Chem.Soc., 39,
(1908) Chem.Zentralbl., I, n.
Tilden, W. A.
(1884) J.Chem.Soc.(Lond.), 45, 269,
409.
Tilden and Shenstone.
(1883) Proc.Roy.Soc.(Lond.), 35, 345
(1884) Phil.Trans., 23-31.
(1885) Proc. Roy. Soc. (Lond.), 38,
331-
Timofeiew, Wladimir.
(1890) Z.physik.Chem., 6, 147.
(1891) Compt.rend., 112, 1137, 1224.
(1894) Dissertation (Kharkhov.)
Timofeiew and Kravtzov.
(1915) Chem.Abs., 9, 2896.
(1917) Chem.Abs., n, 788.
Timmermans, J.
(1907) Z.physik.Chem., 58, 129-213.
(1910) Proc.k.Akad.Wet.(Amst.) 13,
523-
(1911) " Recherches experimentales
sur les phenomenes de
demixtion des melanges
liquides " (These) Brux-
elles. Avril, 1911.
(1912) Bull.soc.chim.(Belg.), 26, 382.
Tinkler, C. K.
(1913) J.Chem. Soc. (Lond.), 103, 2176.
Titherby, A. W.
(1912) Pharm. Jour. (Lond.), 88, 94.
Tobler.
(1855) Liebig's Ann., 95, 193.
Tower.
(1906) Z.anorg.Chem., 50, 382.
Traube.
(1884) Ber., 17, 2304.
Traube, I.
(1909) Ber., 42, 2185, 4185-8.
Trautz and Anschutz.
(1906) Z.physik.Chem., 56, 238.
Treadwell and Reuter.
(1898) Z.anorg.Chem., 17, 185.
Treis, K.
(i9i4)Neues.Jahr.Min.(Beil.Bd.),37,
766-818.
Trevor.
(1891) Z.physik.Chem., 7, 470.
Truthe, W.
(i9i2)Z.anorg.Chem., 76, 129-173.
Tsakalotos, D. E.
(1909) Bull.soc.chim., [4], 5, 397-4°9-
(1910) Jour.chim.phys., 8, 343.
(1912) Bull.soc.chim., 4], 11,287.
(1913) Bull.soc.chim., 4], 13, 282.
(1914) J.chim.phys., 12, 461-3.
Tsakalotos, D. E. and Guye, P. A.
(1910) J.chim.phys., 8, 340.
Tschugaeff, L. A. and Chlopin W.
(Chugaev, L. and Khlopin, W.)
(1914) Z.anorg.Chem., 86, 159.
Tschugaeff, L. A. and Kiltinovic, S. S.
(1916) J.Chem. Soc. (Lond.) 109, 1286.
Tuchschmidt, C. and Follenius, 0.
(1871) Ber., 4, 583.
818
AUTHOR INDEX
Turner, W. E. S. and Bissett, C. C.
(1913) J.Chem.Soc.(Lond.), 103,1904.
Tutton, A. E. H.
(1897) J.Chem.Soc.(Lond.), ?i> 850.
(1907) Proc.Roy.Soc.(LoncL), 79,
(A) 351-82.
Tyrer, Dan.
(1910) Jour.Chem.Soc.(Lond.), 97»
1778-1788.
(igioa) Jour.Chem.Soc.(Lond.), 97,
621-632.
(1911) Proc.Chem.Soc.(Lond.), 27,
142.
Uhlig, J.
(1913) Centr.Min.Geol., 417-22.
Ullik.
(1867) Liebig's Ann., 144, 244.
Umney, J. C. and Bunker, S. W.
> (1912) Perf. Essent. Oil Record, 3,
ioi;4,38.
Unkovskaja, V.
(1913) J.Russ.Phys.Chem.Soc., 45,
x 1099.
u. s. P., vni.
(1907) U. S. Pharmacopoeia, 8th,
decennial revision.
Usher, F. L.
(1908) Z.physik.Chem., 62, 622-5.
(1910) J.Chem.Soc.(Lond.), 97, 66-
78.
Usso.
(1904) Z.anorg.Chem., 38, 419.
Uyeda, K.
(1909-10) Mem. Coll. Sci.Eng. (Ky-
oto), 2, 245-261.
(1912-13) Mem.Coll.Sci.Eng. (Ky-
oto), 5, 147-50.
(1912) 8th Int.Cong.Appl.Chem., 22,
237.
Valenta.
(1894) Monatsh.Chem., 15, 250.
Valeton, J. J. P.
(1910) Verslag k.Akad.Wet.(Amst.),
18, 755- •
Valeur, A.
(1917) Compt.rend., 164, 818-20.
Van de Moer, J.
(1891) Rec.trav.chim., 10, 47.
Vandevelde, A. J. J.
(1911) Bull.soc.chim.(Belg.), 25,210.
Van Eyk, C.
(1899) Z.physik.Chem., 30, 430.
(1900) Proc.k.Akad.Wet.(Amst.), 2,
480.
(1901) Proc.k.Akad.Wet.(Amst.), 3,
98.
(1905) Z.physik.Chem., 51, 721.
(1905) Chem.News., 91, 295.
Van Name, R. S. and Brown, W. G.
(1917) Am.Jour.Sci., [4], 44, 105-23.
Van Slyke, L. L. and Winter, O. B.
(1913) Science, 38, 639.
Vanstone, E.
(1909) J.Chem.Soc.(Lond.), 95, 597.
(1913) J,Chem.Soc.(Lond.), 103,
1828.
(1914) J.Chem.Soc.(Lond.), 105,
1491-1503.
Van't Hofif see van't Hoff.
Van Wyk, H. J.
(1902) Z.anorg.Chem., 32, 115.
(1905) Z.anorg.Chem., 47, 1-52.
Varenne and Pauleau.
(1881) Compt.rend., 93, 1016.
Vasiliev, A. M. (Wasilieff).
(1909) J.Russ.Phys.Chem.Soc., 41,
748-53; 953-7-
(1910) J.Russ.Phys.Chem.Soc., 42,
423, 562-81.
(1910) Chem.Zentralbl.,11, 1527.
(1910) " Tables annuelles," I, 381.
(1911) J.Russ.Phys.Chem.Soc.
(1912) Chem.Abs., 6, 577.
(1912) J.Russ.Phys.Chem.Soc., 44,
1076.
Vaubel.
(1895) J.prakt.Chem., [2], 52, 72.
(1896) Z.physik.Chem., 25, 95.
(1899) J.prakt.Chem., [2], 59, 30.
.(1903) J.prakt.Chem., [2], 67, 472.
Vesterberg, A.
(1912) 8th Inter.Congr.Appl.Chem.,
2, 238, 255.
Vezes, M. and Mouline, M.
(1904) Bull.soc.chim., [3], 31, 1043.
(1905-06) Proc. verb. soc.phys.nat.
(Bordeaux), 123.
Viala, F.
(1914) Bull.soc.chim., [4], 15, 5.
Vignon, Leo.
(1891) Bull.soc.chim., [3], 6, 387, 656.
(1891) Compt.rend., 113, 133.
Virck.
(1862) Chem.Centralbl., 402.
Voerman, G. L.
(1906) Chem.Zentralbl., 77, I, 125.
(1907) Rec.trav.chim., 26, 293.
Vogel, Fritz.
(1903) Z.anorg.Chem., 35, 389.
Vogel.
(1867) Neues Repert.Pharm., 16, 557.
(1874) Neues Repert.Pharm., 23, 335.
Volkhouskii.
(1910) J.Russ.Phys.Chem.Soc., 41,
1763; 42, 1 1 80.
Vortisch, E.
(1914) Neues Jahrb.Min.Geol.(Beilt
Bd.), 38, 185-272.
(19143) Neues Jahrb.Min.Geol.(Beil.
Bd.), 38, 513-24-
Vulpius.
(1893) Pharm.Centralh., 34, 117.
de Waal, A. J. C.
(1910) Dissertation, Leyden.
(1910) " Tables annuelles."
819
AUTHOR INDEX
Waddell, John.
(1898) J.Phys.Chem., 2, 236.
(1899) J.Phys.Chem., 3, 160.
(1900) J.Phys.Chem., 4, 161.
Waentig, P. and Mclntosh, D.
(1916) Trans. Roy.Soc. (Canada), 9,
203^9.
Wagner.
(1867) Z.anal.Chem., 6, 167.
Wagner, C. L.
(1910) Z.physik.Chem., 71, 430.
Wagner, K. L. and Zeraer, E.
(1911) Monatsh.Chem., 31, 833.
Wagemmann, K.
(1912) Metallurgie, 9, 518, 537.
Walden, P. T.
. (1905) Am.Chem.Jour., 34, 149.
(1906) Z.physik.Chem., 55, 712.
Walden, P. T. and Centnerszwer, M.
(1902-03) Z.physik.Chem., 42, 454.
Walker, J.
(1890) Z.physik.Chem., 5, 195.
iWalker, J. and Fyffe, W. A.
(1903) J.Chem.Soc.(Lond.), 83, 179.
Walker, J. and Wood, J. K.
(1898) J.Chem.Soc.(Lond.), 73, 620.
Wallace.
(1855) J.Chem.Soc.(Lond.), 7, 80.
Wallace.
(1909) Z.anorg.Chem., 63, I.
Waller, A. D.
(1904-05) Proc.Roy.Soc.(Lond.), 74,
55-
Walton, J. H. Jr., and Judd, R. C.
(1911) J.Am.Chem.Soc., 33, 1036.
Walton, J. H., and Lewis, H. A.
(1916) J.Am.Chem.Soc., 38, 633.
Wartha.
(1885) Z.anal.Chem., 24, 220.
Warynski, T. and Kourapatwinska, S.
(1916) J.chim.phys., 14, 328-35.
Washburn, E. W. and Maclnnes.
(1911) Z.Elektrochem., 17, 503.
Washburn, E. W. and Read, J. W.
(1915) Proc.Nat.Acad.Sci.(y. S. A.),
i, 191-5-
Wasilieff (see Vasiliev).
Wedekind, E. and Paschke, F.
(1910) Z.physik.Chem., 73, 127.
Wegscheider, R.
(1907) Liebig's Ann., 351, 87.
Wegscheider, R. and Walter, H.
(1905) Monatsh.Chem., 26, 685.
(1907) Monatsh.Chem., 28, 633-72.
Weigel, O.
(1906) Nachr.kgl.Ges.Gottingen, p.
525-48.
(1907) Z.physik.Chem., 58, 293-300.
Weiller, P.
(1911) Chem.Ztg., 35, 1063-5.
von Weimarn, P. P.
(1911) Z.physik.Chem., 76, 218.
Weisberg.
(1896) Bull.soc.chim., [3], 15, 1097.
Wells, H. L.
(1892) Am.Jour.Sci., [3], 44, 221.
Wells, H. L. and Wheeler, H. L.
™(!,892^ Am.Jour.Sci., [3l, 43, 475-
Wells, R. C.
(1915) J.Wash.Acad.Sci., 5, 617-22.
(1915) J.Am.Chem.Soc., 37, 1704.
Wells, R. C. and McAdam, D. J., jr.
(1907) J.Am.Chem.Soc., 29, 721-7.
Welsh, T. W. B. and Broderson, H. J.
(1915) J.Am.Chem.Soc., 37, 816.
Wempe, G.
(1912) Z.anorg.Chem., 78, 298-327.
Wenger.
(1892) Am.Chem.Jour., 16, 466.
Wenger, Paul.
(1911) Dissertation, Geneve.
(1911) " Tables annuelles," 2, 411.
Wentzel.
( ) Dammer's " Handbuch," II,
2, 858.
Wenze.
(1891) Z.angew.Chem., 5, 691.
Werner, E. A.
(1912) J.Chem.Soc.(Lond. ), 101,2169.
Wester, D. H. and Bruins, A.
(1914) Pharm.Weekblad, 51, 1443-6.
Wheeler, H. L.
1892) Am.J.Sci., [3], 44, 123.
1893) Am.J.Sci., [3], 45, 267.
i893a) Z.anorg.Chem., 3, 432.
Wherry, E. T. and Yanovsky, E.
(1918) J.Am.Chem.Soc., 40, 1072.
Whipple, G. C. and Whipple. M. C.
(1911) J.Am.Chem.Soc., 33, 362.
Whitby, G. S.
• (1910) Z.anorg.Chem., 67, 107-9.
Whitney, W. R. and Melcher, A. C.
(1903) J.Am.Chem.Soc., 25, 78.
Wibaut, J. P.
(1909) Chemisch Weekblad, 6, 401.
(1913) Rec.tr.av.chim., 32, 269.
Wigand, A.
(1910) Z.physik.Chem., 75, 235.
Wildeman.
(1893) Z.physik.Chem., n, 421.
Willstaetter.
(1904) Ber., 37, 3753.
Wilsmore.
(1900) Z.physik.Chem., 35, 305.
Wingard, A.
(1917) Svensk.Farm.Tidskrift, 21,
289-93.
(1917) Chem.Abs., u, 2748.
Winkler, L. W.
(1887) J.prakt.Chem., [2], 34, 177;
36, 177-
(1891) Ber., 24, 3609.
(1899) Chem.Ztg., 23, 687.
(1901) Ber., 34, 1409, 1421.
820
AUTHOR INDEX
Winkler, L. W.
(1905) Landolt and Bernstein " Tab-
ellen," 3rd Ed.,- p. 604.
(1906) Z.physik.Chem., 55, 350.
(1912) Landolt and Bornstein " Tab-
ellen," 4th Ed., p. 597, 601.
Winteler, F.
(1900) Z.Elektrochem., 7, 360.
Winterstein, E.
(1909) Arch. exp. Path. u.Pharm., 62,
Wirth, F.
(1908) Z.anorg.Chem., 58, 219.
(1912) Z.anorg.Chem., 76, 174-200.
(1912-13) Z.anorg.Chem., 79, 357.
(1914) Z.anorg.Chem., 87, 1-12.
Wirth, F. and Bakke, B.
(1914) Z.anorg.Chem., 87, 29, 47.
Witt, O. N.
(1915) Ber., 48, 767.
v. Wittorff, N.
(1904) Z.anorg.Chem., 41, 83.
Wolfmann.
(1897) Oster.Ung.Z.Zuckerind., 25,
997-
Wolters.
(1910) N.Jahrb.Min.Geol.(Beil.Bd.),
jo, 57-
Wood, J. Kerfoot.
8) J.<
(1908) J.Chem.Soc.(Lond.), 93, 412.
Wood, J. K. and Scott, J. D.
(1910) J.Chem.Soc.(Lond.), 97, 1573.
Wood, T. B. and Jones, H. O.
(1907-08) Proc. Cambridge Phil.Soc.
14, 171-6.
Worden, E. C.
(1907) J.Soc.Chem.Ind., 26, 452.
Worley, F. P.
(1905) J.Chem.Soc.(Lond.), 87, 1107.
Woudstra, H. W.
(1912) 8th Int.Cong.Appl.Chem., 12,
251-
Wright and Thomson.
(1884-85) Phil.Mag. [5], 17,288; 19, i.
Wright, Thomson and Leon.
(i89i)Proc.Roy.Soc.(Lond.),49, 185.
Wroczynski, A. and Guye, P. A.
(1910) J.chim.phys., 8, 197.
Wroth, B. B. and Reid, E. E.
(1916) J.Am.Chem.Soc., 38, 2322.
Wrzesnewsky, J. B.
(1912) Z.anorg.Chem., 74, 95.
Wuite, J. P.
(1913-14) Z.physik.Chem., 86, 349-
82.
Wiirfel.
(1896) Dissertation, Marburg.
Wiirgler, J.
(1914) Dissertation, Zurich.
Wuth, B.
(1902) Ber., 35, 2415.
van Wyk, see Van Wyk.
Wyrouboff, G.
(1869) Ann.chim.phys., [4], 16, 292.
(1901) Bull.soc.chim., [3], 25, 105,
121.
Yamamoto.
(1908) J.Coll.Sci.(Tokyo), 25, XI.
Young, S. W.
(1897) J.Am.Chem.Soc., 19, 851.
Young, S. W. and Burke, W. E.
(1904) J.Am.Chem.Soc., 26, 1417.
(1906) J.Am.Chem.Soc., 28, 321.
Zaayer, H. G.
(1886) Rec.trav.chim., 5, 316.
Zaharia, A.
(1899) Bul.soc. de sciinte dia Bu-
curesci (Roumania), 8,
53-61-
Zalai, D.
(1910) Gy6gyszereszi Ertesito (Bu-
dapest), 1 8, 366.
(1910) " Tables annuelles," i, 410.
Zambonini, F. F.
(1913) Atti accad.Lincei, [5], 22, I,
523-
Zawidzki, V.
(1904) Z.physik.Chem., 47, 721.
Zemcznzny.
(1908) Z.anorg.Chem., 57, 267.
Zemcznzy and Rambach.
(1910) Z.anorg.Chem., 65, 403.
Zukow, A. and Kasatkin, F.
J.Russ.Phys.Chenl.Soc., 41,
157-66.
821
SUBJECT INDEX
Acenaphthene, I, 2, 16
bromo, 2
chloro, 2
iodo, 2
Acetaldehyde, 2
phenyl hydrazone, 2
trithip, 732
Acetamide, 2
tribromo, 2
trichloro, 2
Acetanilide, 3, 4
chloro and bromo, 4
nitro, 4, 79
oxymethyl, 13
Acetanisidine, 13
Acetic acid, 5-8, 84, 89, 366, 500,
chloro, 5, 9-11
cyano, n
esters, 12
Acetic anhydride, 5
Acetins, mono, di and tri, 13
Acetnaphthalide, 13
Acetone, 13-15, 50, 125, 197, 248,
480, 511,525,534,648,695
phenyl hydrazone, 487
Acetphenetidine, 477
Acetophenol, 89
Acetophenone, 9, 10, 16, 84
amino, 730
Acetotoluidine, 732
Aceturethan, 742
Acetyl acetone, 16
Acetyldiphenylamine, 283
Acetylene, 16, 17, 438
bi iodide, 17
Acetylsalicylic acid, 101, 593
Acetyl tribromophenol, 486
Aconitic acid, 17
Aconitine, 17
Acrylic acid, trichloro, 1 8
Actinium, 18
Adipic acid, 18
Adipinic acid, 18
Adonitol, dibenzal, 698
Agaric acid, 18
Air, 19
Alanine, 19, 20
phenyl, 486
Albumin, 20
Alcohol (Ethyl), 2, 12, 65, 66, 71
125, 126, 160, 163, 235, 239,
247, 248, 286-294, 296, 298-
313, 404-5, 438-9, 466-7, 501,
io, 530, 533, 571, 574, 628,
671
Alizarin, 20
Allantoin, 20
Allocinnamic acids, 254
Allyl alcohol, 511, 534, 647
isothiocyanic ester, 443
mustard oil, 77
thio urea, 738
Aloin, 20
Alums, 30-32, 67, 180, 249, 582, 587,
713
Aluminium bromide, 21-24
chloride, 25-27
fluoride, 27
hydroxide, 28
oxide, 28, 210
626 rubidium alum, 582
sulfate, 29, 31
sulfide, 29
thallium alum, 713
Aminopropionic acid, 19
Aminosuccinic acid, 692
Ammonia, 33-38, 70, 436
444, Ammonium acetate, 39
acid oxalate, 59
acid sulfate, 64
antimony sulfide, 69
arsenates, 39
alum, 30
benzoate, 39
bicarbonate, 41-43
bismuth citrate, 150
borates, 40
bromide, 40, 99, 504
bromide, propyl, benzyl, etc., 41
bromide, tetraethyl, 41
bromide, tetramethyl, 41
cadmium bromide, 41, 167-8
cadmium chloride, 170-1
cadmium iodides, 177
cadmium sulfate, 67
calcium ferrocyanide, 51
calcium sulfate, 214
carbonate, 13, 4^
cerium sulfate, 241, 243
cerium nitrate, 241
chloride, 43, 44-50, 60, 107, 109, 274,
337-8, 353, 643, 7|i
iloru
chloride carnellite, 48
chloride, ethyl and methyl, 50
, 72, chromates, 51
245, chromium alum, 32
300, chromium sulfate, 67
509- citrates, 51
cobalt chlorides, 256
cobalt malonate, 259
822
636,
SUBJECT INDEX
Ammonium acetate, cobalt sulfate,
67
copper chloride, 265-6, 270
copper sulfate, 273, 557
didymium nitrate, 281
fluoboride, 51
fluosilicate, 62
formate, 52
glycyrrhizate, 307
indium sulfate, 67
iodate, 52
iodide, 52
iodide phenyl trimethyl, 55
iodide tetra amyl, 55
iodide tetra ethyl, 53, 55
iodide tetra methyl, 54, 55
iodide tetra propyl, 54, 55
iodomercurate, 55
iridium chlorides, 55, 335
iron alum, 67
iron chloride, 337
iron sulfate, 67
lanthanum nitrate, 347
lanthanum sulfate, 348
lead chloride, 353
lead cobalticyanide, 43
lead sulfate, 67
lithium sulfate, 68
lithium tartrate, 69
magnesium arsenate, 39
magnesium ferrocyanide, 389
magnesium nitrate, 59
magnesium phosphate, 61
magnesium sulfate, 68
manganese molybdate, 59
manganese phosphate, 62
manganese sulfate, 68, 404
mercuric bromide, 406
molybdate, tetra, 55
nickel sulfate, 68, 273
nitrate, 45, 55-60
oleate, 59
oxalate, 59, 376, 735
palmitate, 60
perchlorate, 43, 44
perchlorate derivatives, 44
periodate, 52
permanganate, 62
persulfate, 69
phosphates, 60, 61, 62
phosphites, 62
phosphomolybdate, 55
picrate, 62
platinum bromide, 41
platinum chloride, 498
platinous nitrite compounds, 499
ruthenium nitrosochloride, 587
salicylate, 62
selenate, 62
silico fluoride, 62
sodium phosphates, 62
sodium sulfate, 68
sodium sulfite, 69
Ammonium acetate, sulfate, 45, 56, 60,
63-69, 274, 404, 556, 594
sulfoantmionate, 69
sulfonates, 69
stearate, 63
strontium sulfate, 68
tartrate, 69
tetroxolate, 59
thiocyanate, 35, 70
thorium oxalate, 60, 722
thorium sulfate, 724
trinitrate, 57
urate, 70
uranyl carbonate, 43, 733-4
uranyl nitrate, 735
uranyl oxalate, 735
uranyl propionate, 736
vanadate, meta, 70
vanadium sulfate, 69
zinc chloride, 751
zinc oxalate, 754
zinc phosphate, 754
zinc sulfate, 69, 273
Amygdalin, 70
Amyl acetate, 12, 70, 71
alcohol, 71, 72
alcohol, iso, 71, 72, 291
Amylamine, 72
hydrochloride (iso), 72
Amyl ammonium iodide, tetra, 55
ammonium perchlorates, 44
benzene, 84
benzene (iso), 90
bromide (iso), 292
butyrate, 70
Amylene, 72, 73
hydrate, 73
Amyl ether, (iso), 292
formate, 70, 71
malonic acid, 399
propionate, 70
Andromedotoxine, 73
Anethol, 13, 73
Aniline, 21, 72-80, 88, 89, 443
bromo, 21, 79
dimethyl, 21, 123, 132
ethyl, 79
hydrochloride, 74, 78
methyl, 21, 79, 292
nitro, 4, 78, 79, 80
nitro methyl, tetra, 79
nitroso, 79
nitroso dimethyl, 77, 79
propyl, 79
sulfate, 80
Anisaldehyde, 10
Anisic acid, 80
Anisidine, 80
Anisole, 80, 84, 89
nitro, 80, 421
Anthracene, 81, 82
Anthraflavine, 83
823
SUBJECT INDEX
Anthraquinone, 82, 83
hydroxy, 83
Anthrarufine, 83
Antimony, 83, 705, 712
ammonium sulfide, 69
lithium sulfide, 366, 373
penta chloride, 94
penta fluoride, 94
potassium sulfide, 500-1
potassium tartrate, 96
selenides, 95
sodium sulfide, 627-8
sulfide, 277, 365
tri bromide, 83-88
tri chloride, 88-94
tri fluoride, 95
tri iodide, 95
tri oxide, 95
tri phenyl, 95
tri sulfide, 95
Antipyrine, 4, 96
Apomorphine, hydrochloride, 97, 442
Arabinose, 696
Arachidic acid, 97
Arbutin, 97
Argon, 97
Aribitol, monobenzal, 698
Arsenic, 98, 705, 712
pentoxide, 100
sulfide (ous), 101
tri bromide, 98
tri chloride, 98
tri iodide, 95, 98
tri oxide, 39, 98-100, 629, 642
Asparagine, 101
Asparaginic acid, 101
Aspirin, 101, 593
Astrakanit, 641, 668
Atropine, 101, 102
methyl bromide, 102
Auric, Aurous, (see Gold)
Azelaic acid, 102
Azoanisol, 103
phenetol, 103
Azobenzene, 16, 88, 102, 103, 123, 133,
1 66
amino, 103
hydroxy, 103
Azobenzoic acid ethyl ester, 103
Azolitmine, 104
Azonaphthalene, 103
Azophenetol, 103, 104
Azotoluene, 103
Azoxyanisol, 103
Azoxybenzene, 103
Azoxybenzoic acid ethyl ester, 103
Azoxy phenetol, 103
Barbituric acid, diethyl, 744
Barium acetate, 104
amyl sulfate, 121, 122
arsenate, 104
benzene sulfonates, 122
114
Barium acetate, benzoate, 104
borates, 105
bromate, 105
bromide, 99, 105, 106
butyrate, 106
cadmium chloride, 171
camphorates, 106
cinnamates, 112
citrates, 112
caproate, 107
carbonate, 107, 108, in, 509, 557
chlorate, 108
chloride, 45, 99, 108-111, 643
chromate, in, 112
cyanide, 112
ferrocyanide, 112
fluoride, in, 112
formate, 113
glycerolphosphates, 119
hydroxide, 105, 109, 113,
iodate, 114
iodide, 106, in, 112, 114
iodide mercuric cyanide, 423
iodomercurate, 115
iso caproate, 107
iso succinate, 120
laurate, 120
malate, 115
malonate, 115
molybdate, 115
myristate, 120
nitrate, 45, 55, 109, 113, 115-7, 166,
542
nitrite, 117, 118
oxalate, 118, 119
oxide, 106, in, 119
phenanthrene sulfonates, 122
palmitate, 120
perbromide, 106
perchlorate, 108
periodide, 115
persulfate, 122
picrate, 119
potassium ferrocyanide, 112
propionate, 119
salicylate, 119
salicylate, dinitro, 119
silicate, 119
stearate, 120
succinate, 120
sulfate, in, 120, 121, 509, 557
sulfite, 122
sulfonates, 122
tartrate, 122, 123
truxilate, 123
Behenic acid, 123
methyl ester, 123
Benzalaniline, 123
Benzalazine, 123
Benzaldehyde, 10, 84, 89, 123, 287
trithio, 732
hydroxy, 10
nitro, 10, 123, 124
824
SUBJECT INDEX
Benzaldoxime, 124
nitro, 124
Benzalic compounds of alcohols, 698
Benzamide, 124
Benzanilide, 124
chloro, 124
Benzaniline, 103
Benzazonaphthalene, 103
Benzene, 2, 5, 9, 10, 21, 77* 79, 83, 90,
103, 124, 125-132, 135, 287, 482,
576, 581, 702
bromo, 14, 21, 90, 129, 288, 436, 572
bromochloro, etc., 129
bromo, chloro, iodo, 85
bromo nitro, 23, 24, 26
chloro, 5, 90, 129, 130
chloro, bromo, iodo and fluoro, 128
chloronitro, 22, 23, 25, 77, 128
disulfone chlorides, 130
dibromo, 21, 91
dichloro, 91
ethyl, 85, 90
fluoro, 90
fluoronitro, 85
hexahydro, 280
iodo, 90
isoamyl, 90
mixed halogen substituted, 129, 130
nitro, i, 4, 5, 21, 22, 25, 77, 79, 90, 91,
103, 128, 131, 132,288,303,408,421
nitro chloro, etc., 129, 130
nitroso, 77, 131
propyl, 85, 91
sulfonic acid, 84, 89
tri nitro, 478
Benzhydrol, 128, 132
Benzil, 2, 9, 10, 88, 103, 124, 132, 136
Benzine, 133
Benzoic acid, 5, 9, 10, 77, 84, 89, 128,
I33-H5
amino, 137, 138
amino nitro, 138
bromo, chloro and iodo, 139, 140
chloro, 136, 139
dinitro oxy, 145
fluoro, 136, 140
halogen substituted, 139
iodo, 140
isopropyl, 279
methoxy, 80
methyl, 141
methyl esters, 140
nitro, 136, 141-5, 590
nitro chloro, and bromo, 145
Benzoic aldehyde, nitro, 2
anhydride, 145
Benzoin, 103, 124, 133, 145
Benzonitrile, 21, 84, 90
Benzophenone, 10, 13, 22, 27, 84, 88,
89, 103, 146, 166
tetra methyl diamido, 440
Benzoquinone, 10
Benzosulfonazole, 587-8
Benzosulfonic acids, amino, 136
Benzoyl chloride, 21, 27, 84, 89, 146
Benzoyl phenyl carbinol, 145
phenyl hydrazine, 487
tetra hydroquinaldine, 146
Benzyl acetate, 288
acetone, di, 9
alcohol, 288
Benzylamine, hydrochloride, 147
Benzyl amino succinic acid, 692
Benzylaniline, 123, 145, 147
Benzyl carbamide, 226
chloride, 80
chloride, nitro, 128, 147
ethyl ether, 288
Benzylidene aniline, 124, 145
naphthylamines, 147
Benzylidenes, chloro nitro, 147
Benzyl phenol, 147
Beryllium acetate, 147
fluorides, 148
hydroxide, 148
laurate, 148
meta vanadate, 149
myristate, 148
oxalate, 148
palmitate, 148
phosphate, 148
stearate, 148
sulfate, 148, 149
Betaine, 149
salts, 149
Betol, 149
Bismuth, 150
ammonium citrate, 150
chloride, 150
citrate, 150
double nitrates, 151
hydroxide, 151
iodide, 151
nitrate, 151
oxide, 152
oxychloride, 150
salicylate, 152
selenide, 152
sulfide, 152
telluride, 152
triphenyl, 152
Borax, 629-631 (see Sodium tetra.-
borate)
Boric acid, 40, 153-57, 189, 367, 630
tetra, 157
Boric anhydride, 157
Borneol, 224
Boron trifluoride, 157
Brassidic acid, 158
Brassidinic acid, 123
Bromal hydrate, 158
Bromethyl propyl aceturea, 742
Bromine, 15, 150, 158-62
Bromoform, 128, 162
Brucine, 162
perchlorate, 162
825
SUBJECT INDEX
Brucine, sulfate, 163
tartrate, 163
Butter fat, 302
Butadiene, diphenyl, 163, 254
Butane, 163
Butyl acetate, 12, 163
alcohol, iso, 291
alcohols, 164, 165
ammonium perchlorate, 44
bromide, iso, 292
chloral, 165
chloral hydrate, 165
formate, 163
malonic acid, 399
sulfine perchlorate, 698
Butyric acid, 102, 146, 165-6, 224
trichloro, 166
Butyric aldehyde, 163
Cacodylic acid, 167
Cadmium ammonium bromide,
167-168
ammonium chloride, 170-1
ammonium iodides, 177
barium chloride, 171
bromide, 167
caesium sulfate, 186
chlorate, 169
chloride, in, 167, 169-174
cinnamates, 174
cyanide, 175
fluoride, 170, 175
hydroxide, 175
iodide, 167, 170, 175, 176, 177
magnesium chloride, 171
nitrate, 178
oxalate, 60, 178 ^
potassium bromide, 168
potassium chlorides, 173-4
potassium iodides, 178
potassium sulfate, 179
rubidium bromide, 168
rubidium chloride, 172
rubidium sulfate, 587
silicate, 178
sodium bromide, 169
sodium chloride, 174
sodium iodide, 178
sodium sulfate, 180
sulfate, 170, 178, 179
sulfide, 1 80
Caesium alum, 32, 180
bicarbonate, 181
bromide, 181
carbonate, 181
chlorate, 181
chloraurate, 181
chloride, 182, 183
chromates, 181, 183
cobalt malonate, 259
dihydroxy tartrate, 186
double sulfates, 186
fluoboride, 181
Caesium alum, fluoride, 27, 183
gold chloride, 181, 308
hydroxide, 183
iodate, 183
iodides, 183-4
iridium chlorides, 182
iron chloride, 340
lead bromides, 181
mercuric bromide, 181
mercuric chlorides, 182
nitrate, 184
oxalate, 185
perchlorate, 181
periodate, 183
permanganate, 185
platinum chloride, 182, 498
selenate, 185
sulfate, 185
tartrate, dihydroxy, 186
telluracid oxalate, 185
41, tellurium bromide, 712
tellurium chloride, 182, 712
thallium chloride, 182
uranyl chloride, 734
uranyl nitrate, 735
Caffeine, 186-187
Calcite, 192, 193
Calcium acetate, 187-8 ^
ammomium ferrocyanide, 51
ammonium sulfate, 67, 214
benzoate, 188
bitartrate, 222
borates, 188-9
bromide, 99, 189
bromide mercuric cyanide, 423
butylacetate, 1 88
butyrates, 190
camphorates, 190
caproate, 190
caprylate, 190
carbonate, 191-5, 218
chlorate, 196
chloride, 99, ill, 119, 121, 170, 189,
195-202, 641
chloride acetamidate, 198
chloride acetic acidate, 198
chloride alcoholates, 199
chromates, 199
cinnamates, 200
citrate, 200
ethyl acetate, 188
fluoride, 167, 189, 198, 2OI
formate, 201
glycerophosphate, 2OI
heptoate, 201
hydroxide, 200-5, 215
iodate, 206
iodide, 198, 201, 206
iodo mercurate, 206
lactate, 206
magnesium chloride, 196
malates, 206-207
malonate, 207
826
SUBJECT INDEX
Calcium acetate, methyl acetate, 188
methyl pentanate, 190
nitrate, 203, 207-9, 222
nitrite, 209
oenanthate, 201
oleate, 209
oxalate, 209-10
oxide, 157, 189, 198, 210
pelargonate, 212
perbromide, 189
periodide, 206
phenanthrene sulfonates, 220
phosphates, 210, 211, 212
potassium ferrocyanide, 200
potassium sulfate, 218
propionate, 212
propyl acetate, 188
rubidium sulfate, 218
salicylate, 213
selenate, 213
silicate, 119, 198, 201, 213
sodium thiosulfate, 222
succinates, 213
sulfate, 195, 198, 203, 212, 214-20
sulfate anhydrite, 214
sulfide, 213, 220
sulfite, 220
tartrate,.22i-2
thiosulfate, 208, 222
titanate, 213
valerates, 223
Calomel, 413 (see also Mercurous
chloride)
Camphene, 10, 128, 223
Camphor, 8, 9, 136, 166, 223-5, 593
benzoyl, 224
bromo, 225, 593
chloro, 225
Camphoric acid, 190, 225, 368, 383, 508,
633, 678
anhydride, 225
Camphoroxime, 225
Cane sugar (see Sugar)
Cantharidine, 226
Caoutchouc, 226
Capryl alcohol, 239, 278, 481, 745
Carbamides, 226
Carbazol, 128, 227
Carbinol (see Methyl alcohol)
Carbon dioxide, 227-234, 438
disulfide, 5, 128, 235
monoxide, 235-238
oxysulfide, 238
tetrachloride, 125, 239, 288, 435, 572
Carmine, 239
Carnallite, 388, 641
Carnellite, ammonium chloride, 48
potassium chloride, 48
Carvacrol, 239
Carvoxime, 240
Cascarilla oil, 468
Casein, 2JO
Catechol, 240 «
Cellose, 696
Cephaeline salts, 240
Cerium acetate, 241
ammonium nitrate, 241
ammonium sulfate, 241
butyrates, 241
chloride (ous), 242
citrate, 242
cobalticyanide, 242
dimethyl phosphate, 242
double nitrates, 242
double sulfates, 243
fluoride, 242
formate, 241
glycolate, 242
iodate, 242
malonate, 242
oxalate, 242
propionate, 241
selenate, 243
sulfate, 243-4
sulfonates, 244
tartrate, 244
tungstate, 244
Cesium, (see Caesium)
Cetyl alcohol, 9, 244, 574
Chloral formamide, 245
hydrate, 96, 244-5 ,
Chlorine, 15, 150, 160, 239, 245-7
dioxide, 247
monoxide, 247
trioxide, 247
Chloro acetic acid esters, 12
Chloroform, 14, 15, 77, 126, 131, 247
248, 289, 435, 571
Cholesterol, 248-9
acetate, 248
digitonide, 248
stearic acid ester, 249
Cholesteryl benzoate, 103
isobutyrate, 103
propionate, 103
Choline perchlorate, 249
Chromic acid, 51, 250, 372, 584, 651
Chromium alums, 249
ammonium alum, 32
ammonium sulfate, 67
caesium alum, 180
chlorides, 249, 250
double salts, 250
nitrates, 250
sulfates, 250
thiocyanate, 250
potassium cyanide, 531
potassium thiocyanate, 531
rubidium alum, 582
thallium alum, 713
trioxide, 183, 250
Chrysarobin, 250
Chrysene, 250
Cineole, 251
Cinchona alkaloids, 251
827
SUBJECT INDEX
Cinchonidine, 251
salts, 252
Cinchonine, 251
salts, 252
Cinchotine salts, 252
Cinnamic acid, 9, 10, 136, 252-254
bromo, 253, 254
chloro, 254
methoxy, 254
Cinnamic aldehydes, chloro and bromo,
254
Cinnamylidene, 123, 147, 163, 254
acetophenone, 16
Citric acid, 51, 254-55
Cobalt acetate, 256
amines, 255
ammonium chlorides, 256
ammonium sulfate, 67 -
bismuth nitrate, 151
bromide, 256
caesium sulfate, iS6
cerium nitrate, 242
chlorate, 256
chloride, 45, 256-8
citrates, 258
double salts, 255
fluoride, 258
gadolinium nitrate, 304
iodate, 258
iodide, 258
lanthanum cyanide, 346
lanthanum nitrate, 347
lead cyanide, 357
malate, 259
malonates, 259
neodymium cyanide, 449
neodymium nitrate, 449
nitrate, 259
oxalate, 259
perchlorate, 256
potassium citrate, 258
potassium sulfate, 557
praseodymium nitrate, 568
rubidium nitrite, 259
rubidium sulfate, 587
samarium nitrate, 594
sulfate, 259-60
sulfide, 260
thallium cyanide, 717
ytterbium cyanide, 746
. yttrium cyanide, 746
Cocaine, 261
• hydrochloride, 261
perchlorate, 261
Cocaline, 302
Codeine, 261
phosphate, 261
sulfate, 261
Colchicine, 262
salts, 262
Collidine, 262
Congo red, 262
Coniine, 262
Copiapite, 344
Copper acetate, 262-3
ammonium chloride, 265-6, 270
ammonium sulfate, 273, 557
bromide, 167, 263
caesium sulfate, 186
carbonate, 263-4
chlorate, 264
chloride, 109, in, 150, 264-270,
274
chloride (ous), 170, 183, 198
cyanide, 270, 531
hydroxide, 270
iodate, 271
iodide, 177, 271
manganese sulfate, 403
nitrate, 271, 360
oxalate, 272
oxide, 270, 272
potassium carbonate, 264
potassium chloride, 267-8, 270
potassium sulfate, 274, 557
rubidium sulfate, 587
sodium sulfate, 276
- sulfate, 63, 272-7, 403, 454
sulfide, 95, 277
sulfonates, 277
thallium sulfate, 720
tartrate, 277
thiocyanate, 278
Cotton seed oil, 294, 436, 468
Coumarin, 132, 278
Cream of tartar, 564-566
Cresol, 9, 10, 77, 128, 251, 278, 279
trinitro, 279
Crotonic acid, 9, 10, 279
chloro, 279
Cryolite, 28
Cumidine, pseudo, 279
Cuminic acid, 279
Cyanimide, 279
Cyanogen, 280
Cyclohexane, 5, 86, 91, 128, 280
Cyclohexanol, 280
Cyclohexanone, 280
Cymene, 85, 91
pseudo, 86
Cryptopines, methyl, 279
Cytisine, 280
Detonal, 742
Dextrin, 281
Diacetyl morphine, 442
Diacetyl racemic ether, 281
tartaric ether, 281
Diamine mercuric chloride, 419
Dibenzyl, 103, 123, 133, 145, 147, 281
acetone, 9
hydrazine, 147
Dibnal, 742
Dicyandiamidine, 279
Didymium ammonium nitrate, 281
potassium sulfate, 281
828
SUBJECT INDEX
Didymium sulfate, 281
sulfonates, 281
Diethylamine (see Ethyl amine), 281
Diethylbarbituric acid, 742, 744
Diethyldiacetyl tartrate, 131
Diethylene ether, 302
Diethylketone, 289
Diethyl oxalate, 10
Dihydro naphthoic acids, 447
Dimethoxystilbene, 103
Dimethyl amine (see Methyl amine) , 437
malonate, 10
oxalate, 9, 10
pyrone, 5, 9, 10, 21, 132, 136, 143,
1 66, 253, 279, 304, 346, 400, 448,
484, 486, 495, 575
succinate, 5, 9, 10
terephthalate, 10
urea, 484
xanthine, 721
Dionin, 281, 442
Diphenyl, 86, 91, 128, 282
acetylene, 123, 254
amine, 130, 132, 282-3
amine blue, 283
amine, hexanitro, 283
butadiene, 123
imide, 227
hydrazine, 123
methylamine, 283
oxide, 282
selenide, 283
sulfide, 283
telluride, 283
urea, 738
Dipyridyl 77, 132
Dipronal, 742
Dipropylazophenetol, 103
Double mercuric chlorides, 420
Dulcitol, dibenzal, 698
Dyes, 283
Dysprosium oxalate, 283
Edestin, 283
Egg albumin, 20
Elaterin, 284
Emetine and salts, 284
Epronal, 742
Erbium dimethyl phosphate, 284
oxalate, 284
sulfate, 284
sulfonate, 284
Erusic acid, 123, 158, 284
Erythritol, 284, 698
dibenzyl, 698
Eserine, 492
Ethane, 285
Ethane, diphenyl, 88
Ether, ethyl, 5, 10, 15, 16, 83, 128, 131,
247, 248, 282, 289-290, 295, 297-9,
313, 323, 425, 541
petroleum, 477
Ethyl acetate, 10, 12, 77, 160, 247,
285-6, 290, 313
Ethyl alcohol (see Alcohol)
amine, di, 128
amine hydrochloride, 296
amine, tri, 102, in, 133, 224, 405
amines, 294-6
ammonium bromide, tetra, 41
ammonium chloride, tetra, 50
ammonium iodide, tetra, 53, 55
ammonium perchlorates, 44
benzene, 90
benzoate, 10
bromide, 160, 290, 296, 436, 572
butyrate, 290, 296
carbamate, 296, 741-2
chloracetate, 12
diacetyl tartrate, di, 300
dichlor acetate, 12
Ethylene, 301
bromides, 5, 22, 79, 103, 128, 131,
280, 281, 283, 300, 301, 431
chlorides, 128, 291, 296
cyanide, 302, 693
tetraphenyl, 302
Ethyl ether (see ether)
formate, 299
Ethylidene chloride, 291, 296
Ethyl iodide, 296
ketone, di, 300
malonic acid, 399
methyl ketone, 299, 534, 649
morphine, 281, 442
morphine hydrochloride, 443
piperidine, 496
propionate, 290, 300
succinimide, 693
sulfine perchlorate, 698
sulfonium iodide, tri, 699
sulfon methanes, 435
trichlor acetate, 12
Ethyl urethan, 742
valerates, 300
Eucaine and salts, 302
Eucalyptole, 251
Europium sulfonate, 302 '
Fats, 302
Fatty acids, 468
Ferric (see Iron)
Ferrous (see Iron)
Fluorene, 132, 145, 303
Fluorenone, 132
Fluorescein, 303
Formaldehyde, 303
Formamide, 5, 166, 303
Formanilides, chloro, 303
Formic acid, 5, 126, 130, 303, 304
Fruit sugar, 695-7
Fumaric acid, 304
Furfuralazine, 123
Furfurol, 304
829
SUBJECT INDEX
Gadolinium cobalticyanide, 304
dimethyl phosphate, 305
double nitrates, 304
glycolate, 304
oxalate, 304-5
sodium sulfate, 305
sulfate, 305
sulfonates, 305
Galactose, 305, 695-7
Gallic acid, 305-6
Germanium dioxide, 306
potassium fluoride, 535
sulfide, 306
Glass, 306
Glaserite, 559, 641
Globulin, 306
Glucoheptose, 696
Glucose, 306, 695-97
Glutaminic acid, 306
hydrochloride, 307
Glutaric acid, 307
Glycerol, 75, 125
Glycine, in, 307
Glycocoll, 307
trimethyl, 149
Gly colic acid, 307
phenyl, 307
Glycyrrhizic acid, 307
Gold, 308, 705, 712
caesium chloride, 181
chloride, 308
double chlorides, 308
lithium chloride, 369
phosphorus trichloride, 308
Grape sugar, 695-97
Guaiacol, 251, 309
carbonate, 309
Guanidine, triphenyl, 2, 309
Gulose, 697
Gun cotton, 465
Helianthin, 309
Helium, 309-310
Hemoglobin, 309
Heptane, 239, 278, 291, 310, 436, 481
Heptpic acid, ^3 10
Heroine, 442
Hexahydrobenzene, 280
Hexamethylene, 280
tetramine, 310
Hexane, 78, 131, 291, 310, 436
Hexanitrodiphenylamine, 283
Hippuric acid, 310-11
Holocaine hydrochloride, 311
Homatropine hydrobromide, 311
Hydrastine, 311
Hydrastinine hydrochloride, 311
Hydrazides, 312
Hydrazine, 312
dibenzyl, 147
nitrate, 312
perchlorate, 312
sulfate, 312
Hydrazobenzene, 103, 123, 145, 147
Hydriodic acid, 312
Hydrobenzene, 103, 147
tetra, 87
Hydrobenzoic acids, hexa, 140
Hydrobenzoin, 133
Hydrobromic acid, 15, 160, 248, 313
Hydrochloric acid, 247, 248, 298, 313-5,
517, 649
Hydrocinnamic acid, 253, 570
Hydrocyanic acid, 315
Hydrofluoric acid, 315
Hydrogen, 316-21
peroxide, 321-2
selenide, 322
sulfide, 37, 313, 315, 322-3
Hydroquinol, 15, 77, 103, 224, 251, 254,
323-4
chloro and bromo, 324
diacetyl chloro and bromo, 324
Hydroquinone (see Hydroquinol)
Hydroxy benzaldehyde, 123
benzoic acids, 140, 141
benzoic acid, dinitro, 145
Hydroxylamine, 324
hydrochloride, 324
Hyoscine hydrobromide, 325
Hyoscyamine, 324
Hypophosphoric acid, 490
Iditol, tribenzal, 698
Indan carboxylic acid, nitro, 325
Indigo, 325
Indium ammonium sulfate, 67
caesium alum, 180
iodate, 325
Inositol, iso, 325
lodic acid, 325, 536, 654
Iodine, 55, 95, 98, 150, 160, 184, 206,
247, 271, 325-34, 429, 537, 713
lodoeosine, 335
lodoform, 335
lodol, 335
Iridium ammonium chlorides, 55, 335
caesium chlorides, 182
chloride, 335
double salts, 335
potassium chloride, 526
rubidium chlorides, 585
Iron ammonium sulfate (alum), 67
bicarbonate, 336
bromide (ous), 335
caesium alum, 180
caesium chloride, 340
caesium sulfate, 186
carbonate (ous), 336
chloride, 150, 267, 270, 336-40
fluoride, 652
formate 340
hydroxide, 341, 342
nitrate, 341
oleate, 342
oxalate, 342
830
SUBJECT INDEX
Iron ammonium sulfate (alum), oxide,
210, 342
phosphates, 342
potassium chloride, 339-40
potassium sulfate, 345, 558
rubidium alum, 582
rubidium sulfate, 587
sodium sulfate, 344
sulfate, 29, 64, 179, 343-45
sulfide, 277, 342, 345
sulfonates, 345
thallium alum, 713
thallium cyanide, 717
thiocyanate, 345
Isoamyl alcohol, 574
urethan, 742
Isobehenic acid, 123
Isobutyl acetate, formate, etc., 163
alcohols, 164-5, 574
Isobutylamine hydrochloride, 165
Isobutyric acid, 165-6
Isoerusic acid, 123
Isopentane, 77, 476
Isophthalic acid, 490
Isopropyl aicohol, 511, 533, 571
amine, 573
bromide, 573
chloride, 573
iodide, 573
Itaconic acid, 345
Kainite, 641
Keratin, 345
Kieserite, 641
Krypton, 345
Lactdiethylamide, 744
Lactic acid, 125, 346
trichloro, 346
Lactose, 695-97
Lanthanum ammonium nitrate, 347
bromate, 346
citrate, 346
cobalticyanide, 346
dimethyl phosphate, 348
double nitrates, 347
double sulfates, 348
glycolate, 346
iodate, 346
malonate, 346
molybdate, 347
oxalate, 347
sulfate, 348
sulfonates, 348
tartrate, 349
tungstate, 349
Laurie acid, 349
Lead, 349, 705, 712
acetate, 349-350 ^
ammonium chloride, 353
ammonium cobalticyanide, 43
ammonium sulfate, 67
arsenate, 350
Lead, benzoate, 351
borate, 351
bromate, 351
bromide, 150, 351-2
caesium bromides, 181
caprate, 352
caproate, 352
caprylate, 352
carbonate, 352-3
chlorate, 353
chloride, 46, III, 150, 170, 198, 270,
339, 351, 353-56
chromate, 353, 357
citrate, 357
diphenyl dicyclohexyl, 352
double cyanides, 357
ferricyanide, 357
fluoride, 351, 356, 357
fluoro chloride, 356
formate, 358
heptylate, 352
hexyl bromide, 352
hexyl chloride, 352
hydroxide, 358
hyposulfate, 365
iodate, 358
iodide, 351, 356, 357, 358, 359
laurate, 352, 360
malate, 359
myristate, 352
nitrate, 116, 360-2
Lead nonylate, 352
oxalate, 362
oxides, 351, 356, 357, 362
palmitate, 352, 360, 362
peroxide, 362
persulfate, 365
phosphate, 357, 362
potassium chloride, 355
potassium ferricyanide, 357
potassium iodide, 359
potassium sulfate, 364, 558
stearate, 352, 360, 362
succinate, 363
sulfate, 357, 362-65
sulfide, 95, 277, 345, 356, 365
sulfonates, 365
tartrate, 366
tetraphenyl, 352, 362
tetracyclohexyl, 352
Lecithin, 366
Leonite, 641
Leucine, 366
Lignoceric acid, 97, 366
Ligroin, 366
Lime (see Calcium hydroxide)
Linseed oil, 468
Lithium, 37, 366
acetate, 366
ammonium sulfate, 68
ammonium tartrate, 69
antimony sulfide, 366, 373
benzoate, 367
831
SUBJECT INDEX
Lithium, bicarbonate, 369
bichromate, 372
borate, 367
bromate, 367
bromide, 100, 367
camphorate, 368
carbonate, 368-9
chlorate, 369
chloraurate, 369
chloride, 100, in, 183, 198, 270, 356,
370-1
chromate, 372
citrate, 372
fluoride, 27, 373
formate, 373
gold chloride, 308, 369
hippurate, 373
hydroxide, 367, 371-3
hypophosphate, 377
iodate, 374
iodide, 373, 374
lodo mercurate, 374
laurate, 374, 375
mercuric iodide, 374
molybdate, 375
myristate, 374, 375
nitrate, 117, 376
nitrite, 376
oleate, 374
oxalate, 60, 376
oxide, 378
palmitate, 374, 375
permanganate, 377
phosphate, 377
potassium sulfate, 377
salicylate, 377
silicate, 119, 213, 367, 378
sodium sulfate, 377
stearate, 374, 375
sulfate, 29, 64, 121, 179, 220, 259,
274, 343, 365, 369, 376, 377, 378
sulfoantimonate, 366, 373
tartrates, 378
Lutidine, 574
Lyxose, 696
Magnesium, 378
acetate, 378
ammonium arsenate, 39
ammonium ferrocyanide, 389
ammonium nitrate, 59
ammonium phosphate, 61
ammonium sulfate, 68
benzoate, 379
bicarbonate, 385-86
bismuth nitrate, 151
bromate, 379
bromide, 379
bromide alcoholates, 379, 381
bromide anilinates, 379, 381
bromide compounds, 379, 382-3
bromide etherate, 379-80
Magnesium, bromide phenylhydrazi-
nates, 379, 382
cadmium chloride, 171
caesium sulfate, 186
calcium chloride, 196
camphorate, 383
carbonate, 13, 384-86
cerium nitrate, 242
chlorate, 387
chloride, 46, in, 170, 196, 198, 339,
356, 371, 387-8, 641
cinnamate, 389
chromate, 389
ferrocyanides, 389
fluoride, 389
fluosilicate, 396
gadolinium nitrate, 304
hydroxide, 385, 389, 390
hypophosphate, 395
iodate, 390
iodide, 390
iodide alcoholates, 391, 392
iodide anilinates, 391, 392
iodide compounds, 391, 393, 394
Magnesium iodide etherates, 391, 392
iodo mercurate, 394
lanthanum nitrate, 347
laurate, 394
mercuric iodide, 394
myristate, 394
neodymium nitrate, 449
nitrate, 395
oleate, 395
oxalate, 60, 395
oxide, 28, 210, 378, 395
palmitate, 394
phosphate, 395
platinic cyanide, 389
potassium ferrocyanide, 389
potassium chloride, 388
potassium chromate, 389
potassium sulfate, 396, 397
praseodymium nitrate, 568
rubidium sulfate, 587
salicylate, 395
samarium nitrate, 594
silicate, 213, 378, 396
sodium sulfate, 668
stearate, 394
succinate, 396
sulfate, 273, 388, 396-7, 480, 641, 668
sulfite, 397
sulfonates, 397
Maleic acid, 304, 398
Malaminic acid, 398
Malonic acid, 299, 398-9
Malonic acids, substituted, 399
Maltose, 695-7
Mandelic acid, 398-400
butyl esters, 400
methyl esters, 400
Manganese ammonium molybdate, 59
ammonium phosphate, 62
832
SUBJECT INDEX
Manganese ammonium molybdate, am-
monium sulfate, 68, 404
bismuth nitrate, 151
borate, 400
bromide, 400
caesium sulfate, 1 86
carbonate, 401
cerium nitrate, 242
chloride, 47, in, 170, 198, 356, 371,
388, 401
cinnamate, 401
copper sulfate, 403
fluosilicate, 401
hydroxide, 401-2
hypophosphite, 402
iodomercurate, 402
lanthanum nitrate, 347
mercuric iodide, 402
neodymium nitrate, 449
nitrate, 402
oxalate, 402
oxide, 402
potassium chloride, 401
potassium vanadate, 405
praseodymium nitrate, 568 .
rubidium sulfate, 587
samarium nitrate, 594
silicate, 119, 213, 396, 402
sodium sulfate, 404
sulfate, 274-5, 378, 403-5
sulfide, 405
titanate, 402
Mannitol, 166, 405, 698
tribenzal, 698
Mannose, 695-7
Matico oil, 468
Mellibose, 696
Mellitic acid, hexamethyl, 431
Menthane, 431
Menthol, 128, 131, 224, 245, 431
Menthyl mandelates, 400
Mercury, 378, 598
acetate, 406
ammonium iodide, 55
barium iodide, 115
benzoate, 406
bromide, 131, 158, 351, 406-8
caesium bromide, 181
caesium chlorides, 182
calcium iodide, 206
chloride, 47, 80, no, 182, 268,
409-21, 526
cinnamate, 422
cyanide, 422-4
diphenyl, 95, 152, 430
double cyanides, 423
fulminate, 424
iodide, 170, 177, 408, 421, 424-9, 616
iodide diamine, 429
lithium iodide, 374
magnesium iodide, 394
manganese iodide, 402
nitrate, 429
Mercury, oxide, 429-30
potassium chloride, 410, 420
potassium iodide, 425, 541
rubidium chloride, 412
selenite, 430
sodium chloride, 411
sodium iodide, 656
strontium iodide, 682
sulfate, 430-1
sulfide, 431
zinc thiocyanate, 752
Mesitylene, 86, 92, 292
Meta arsenic acid, 98
Methacetin, 13
Methane, 432-3
diphenyl, 86, 92, 433
triphenyl, 88, 282, 309, 433-4
Methoxybenzoic acid, 80
Methoxycinnamic acid, 103
Methoxystilbene, di, 677
Methyl acetate, 12, 247, 435
alcohol, 5, 37, 72, 128, 160, 235, 247,
248, 280, 286, 299, 313, 315, 323,
435, 436, 501 , 5i°. 574
amines, 437, 438
amine chloroplatinates, 438
amine hydrochloride, 438
ammonium bromide, tetra, 41
ammonium chloride, tetra, 50
ammonium iodide, tetra, 54, 55
ammonium perchlorates, 44
aniline, 21, 292
aniline, di, 132
anisate, 10
benzoate, 10, 21
benzoic acids, 730
Methylene blue, 439
bromide, 21, 439
Methyl butyrate, 438
carbinol, tri, 227
chloride, 315, 439
cinnamate, 9, 10
cryptopines, 279
ether, 37, 248, 301, 315, 438
ethyl ketone, 299, 534, 649
hexyl carbinol, 574
iodide, 436, 439
iso thiocyanate, 443
malonic acid, 399
mellitic acid, hexa, 431
mustard oil, 223
orange, 309, 459
oxalate, 439
phenyl carbamide, 226
phenyl picramides, 492
picric acid, 495
piperidines, 496
propionate, 439
propyl azo phenol, 103
pyridines, 574
pyridines, tri, 262
pyridine zinc chloride, 574
salicylate, 251, 439
833
SUBJECT INDEX
Methyl butyrate, succinic acid, 711-2
sulfate, 440
sulfine perchlorate, 698
sulfone methanes, 435
toluate, 10
urea, 484
urethan, 431, 742
valerate, 438
Michler's ketone, 440
Milk sugar, 695^-97
Molybdenum trioxide, 440
Molybdic acid, 440
Morphine, 441
acetate, 442
hydrochloride, 442
perchlorate, 442
salts, 442
sulfate, 442
tartrate, 442
Mustard oil, 443
Myristic acid, 443
Naphthalene, 5, 9, 13, 21, 79, 86, 92,
98, 123, 128, 130-2, 166, 223-4,
251, 279, 282-3, 300-1, 324, 431,
433-4, 443-7
bromo, 87, 92
chloro, 87, 92
dihydro, 446
nitro, 86, 92, 224, 283, 408, 421, 446
picrate, 126
sulfonic acid, 446
Naphthoic acid, 447
Naphthoic acids, dihydro, 447
Naphthols, 10, 128, 224, 251, 283, 301,
446, 447, 448, 593, 703,
Pirate 447
Naphthyl acetate, 10
amine, 79, 224, 240, 283, 309, 446,
448
amine sulfonic acids, 448
benzoate, 448
hydrazones of sugars, 697
salicylate, 149
Narceine, 448
Narcotine, 449
Neodymium chloride, 449
cobalticyanide, 449
dimethyl phosphate, 450
double nitrates, 449
glycolate, 449
molybdate, 449
nitrate, 450
oxalate, 449-50
sulfonates, 450
tungstate, 450
Neon, 450
Neurine perchlorate, 450
Nickel ammonium sulfate, 68, 273
bismuth nitrate, 151
Nickel bromate, 451
bromide, 451
caesium sulfate, 186
Nickel bromate, carbonate, 451
car boxy 1, 451
cerium nitrate, 242
chlorate, 451
chloride, 47, 452
citrate, 452
gadolinium nitrate, 304
hydroxide, 452
iodate, 452
iodide, 453
lanthanum nitrate, 347
malate, 453
neodymium nitrate, 449
nitrate, 453
oxalate, 453
perchlorate, 451
potassium citrate, 452
potassium sulfate, 455, 557
praseodymium nitrate, 568
rubidium sulfate, 587
samarium nitrate, 594
sodium sulfate, 454
sulfate, 453-5
sulfide, 455
thallium sulfate, 720
Nicotine, 456
Nigella oil, 468
Niobium potassium fluoride, 456
Nitric acid, 224, 395, 456-7, 542
oxide, 438, 461, 465
Nitrocellulose, 465
Nitrogen, 457-461
oxide (ic), 461
oxide (ous), 462-5
tetroxide, 465
Nitrophenyl chloroform, 248
Nitrosobenzene, 131
Nitrosopiperidine, 496
Nitrosyl chloride, 247
Nitrous oxide, 462-5
Novocaine, 466
hydrochloride, 466
Octane, 466
Octyl alcohol, 239, 278, 481, 745
Oenanthyl urethane, 742
Oils, 302, 468
baldo leaves, 468
castor, oleic, olive, etc., 249
cotton seed, 294, 436
helianthus annus, 468
olive, 468
turpentine, 440, 733
Oleic acid, 248, 466-7
Olein, tri, 467
Orthovanillin, 744
Osmic acid, 468
Oxalic acid, 59, 185, 348, 376, 468-9
549-51, 66 1
Oxybenzoic acids, 140, 141, 251
Oxybenzoic acid, dinitro, 145
Oxygen, 470-3
834
SUBJECT INDEX
Ozokerite paraffin, 475
Ozone, 473-4
Palladium chloride, 474
Palmitic acid, 97, 248, 443, 467, 474~5,
677
acetic ester, 446
acid cetyl ester, 475
Palmitin, tri, 467, 475
Papaverine, 475
Paraffin, 283, 446, 475
Paraformaldehyde, 303
Paraldehyde, 2, 128, 301
Para morphine, 721
Pentane, 476
iso, 77, 131, 282
Peptone, 476
Perchloric acid, 476
Perseitol, dibenzal, 698
Petroleum, 294
benzine, 133
ether, 477
Phenacetin, 477
Phenanthraquinone, 477-8
Phenanthrene, 128, 132, 145, 223, 282,
283, 443, 478-79
picrate, 479
Phenetidine, acet, 477
Phenetol, 86, 93, 292
dinitro, 80
Phenol, 9, 10, 15, 76, 78, 79, 83, 86, 93,
102, 123, 124, 127, 131-3. 135, H6,
156, 224, 227, 251, 280, 283, 295,
300, 301, 310, 315, 373, 397, 423,
433, 445, 446, 448, 466, 479-84,
536, 682, 704
dinitro, 4, 303
Phenols, amino, 136, 251
acetyl tribromo, 486
bromo, 484, 486
chloro, 15, 77, 79, 283, 486
iodo, 486
nitro, 15, 77, 128, 251, 446, 484-6
nitroso, 486
tribromo, 132
Phenolate of phenyl ammonium, 484
Phenolphthalein, 486
Phenyl acetic acid, 9, 12
alanine, 486
amine, di, 21, 80, 128, 282-3
amine, tri, 282
anisyl ketone, 10
benzoate, ip
carbinol, tri, 227
diacetylene, di, 163
dibromo propionic acid, 570
Phenylene diamines, 486
Phenyl ether, 132
ethylene, tetra, 302
glycolic acid, 307
glyoxal phenyl hydrazone, 307
guanidine, tri, 2, 309
hydracrylic acid, 732
Phenyl hydrazines, 484, 486-7
hydrazine, di, 163
hydrazones of sugars, 697
methane, di, 433
methane, tri, 282, 309, 433-4, 704
methyl amine hydrochloride, 438
methyl carbamide, 226
piperidines, di, 497
propiolic acid, 570
propionic acid, 254, 570
salicylate, 10, 251, 593
selenide, dibromo, 487
selenium bromide, di, 596
telluride, dibromo, 487
tellurium bromide, di, 596
thiocarbamide, 738-9, 740
thio urea, 738-740
trimethyl ammonium iodide, 55
Phloroglucinol, 487
Phosphomolybdic acid, 488
Phosphoric acid, 224, 489-90
Phosphorus, 488-9
acid, 489
sulfides, 489
triiodide, 95, 98
Phthalic acids, 490
Phthalic acids, nitro, 491
Phthalic anhydride, 491
Phthalide, 2, 309
carbpxylic acid, 492
Phthalimide, 492
Phthalonic acid, 492
Phthalyl hydroxylamine 324
phenyl hydrazides, 312, 487
Physpstigmine, 492
salicylate, 492
sulfate, 492
Phytosterol, 248
Picramides, methyl phenyl, 492
Picric acid, 5, 81, 240, 279, 301, 303,
309, 446-8, 484, 486, 492-5, 731
methyl, 495
Picrotoxine, 495
Picoline, 574
Pilocarpine, 496
hydrochloride, 496
nitrate, 496
Pinacplin, 496
Pimelic acid, 495
Pinene, 293
hydrochloride, 496
Pipecoline, 496
Piperidine, 280, 496
propyl, 262
Piperidines, di phenyl. 497
Piperidine hydrochloride, 496
methyl, 496
Piperine, 496, 497
Piperonal, 9, 10, 136
nitro, ID
Piperonilic aldehyde, 2
Platinates, chloro, of hydrocarbon sul-
fines, 499
835
SUBJECT INDEX
Platino amines, 499
Platinous nitrite ammonium com-
pounds, 499
Platinum alloys, 497
ammonium bromide, 41,
bromide, 497
caesium chloride, 182
chlorides, 499
double chlorides, 498
magnesium cyanide, 389
potassium bromide, 497
Ponceau, 499
Potasammonium, 500
Potassium, 37, 500
acetate, 500
acid sulfates, 560
alum, 30, 31
amyl sulfate, 564
antimony sulfide, 500-1
antimony tartrate, 96
arsenate, 501
barium ferrocyanide, 112
benzoate, 502
beryllium fluoride, 148
bicarbonate, 508-9
bioxalate, 551
bisulfate, 560, 563
bitartrate, 564-6
bitartrate, dimethyl ester, 566
borates, 502
bromate, 503
bromide, 100, 167, 263, 480, 504-7
bromide, mercuric cyanide, 423
butyrate, 508
cadmium bromide, 168
cadmium chlorides, 173-4
cadmium iodides, 178
cadmium sulfate, 179
calcium ferrocyanide, 200
calcium sulfate, 218
camphorates, 508
carbonate, 13, 35, 264, 353, 369,
508-12, 544, 557
carbonyl ferrocyanide, 531
cerium sulfate, 243
chlorate, 512-15, 714
chloride, 45, 48, 109, in, 121, 170,
174, 183, 196, 198, 267, 270, 274,
307, 339, 340, 356, 371, 388, 410,
480, 504, 505, 507, 509, 512, 516-
26, 531, 543, 552, 637, 641, 643,
668, 672
chloride, carnellite, 48
chloride mercuric cyanide, 423
chloro iridate, 526
chloro platinate, 498
chromate, 353, 526-30, 559
Potassium chromium alum, 249
chromium molybdate, 250
chromithiocyanate, 531
chromocyanide, 531
citrate, 530
cobalt citrate, 258
Potassium chromium alum, cobalt mal-
onate, 259
cobalt sulfate, 557
copper carbonate, 264
copper chloride, 267-8, 270
copper sulfate, 274, 557
cyanate, 531
cyanide, 270, 531
dichromate, 527-30
didymium sulfate, 281
dihydroxy tartrates, 566
dipropyl malonate, 512
ethyl sulfate, 563-4
ferricyanide, 531-2
ferrocyanide, 531-2
ferrosulfate, 558
fluoboride, 502
fluoride, 27, 112, 242, 507, 526, 532-4
fluotitanate, 568
formate, 535
germanium fluoride, 535
gold chloride, 308
hippurate, 311
hydroxide, 501, 502, 507, 509, 526,
529, 534-6, 555, 558
hypophosphate, 555
hypophosphite, 555
iodate, 536
iodide, 100, 177, 326, 425, 504, 505,
507, 518, 519, 526, 534, 536,
iodide
lide mercuric cyanide, 423
iodomercurate, 541
iridium chloride, 526
iron chloride, 339-40
iron sulfate, 345
lanthanum sulfate, 348
lead chloride, 355
lead cobalticyanide, 357
lead ferricyanide, 357
lead iodide, 359
lead sulfate, 364, 558
lithium sulfate, 377
lithium tartrate, 378
magnesium chloride, 388
magnesium chromate, 389
magnesium ferrocyanide, 389
magnesium sulfate, 396, 397
manganese chloride, 401
manganese sulfate, 405
mercuric cyanide, 423
mercuric chloride, 410-11, 420
mercuric iodide, 425, 541
meta borate, 502
meta phosphate, 502, 526, 534, 555
methyl sulfate, 564
molybdate, 529, 530, 541
nickel citrate, 452
nickel sulfate, 455, 557
niobium fluoride, 456
nitrate, 45, 55, 116, 117, 208, 360,
376, 480, 506, 509, 519, 520, 521,
541, 542-8, 552, 643, 657, 659, 718
836
SUBJECT INDEX
Potassium chromium alum, nitrite,
548-9
oxalate, 60, 549-52, 735
perborates, 502
perchlorate, 515, 554
periodate, 536
permanganate, 552-4
persulfate, 563
phosphates, 526, 534, 554-5
phosphomolybdate, 555
picrate, 554, 719
platinum bromide, 497
platinum chloride, 498
pyrpphosphate, 526, 534, 555
rubidium perchlorate, 583
rubidium nitrosochloride, 587
selenate, 556
silicate, 378, 556
sodium carbonate, 512
sodium sulfate, 668, 559
sodium sulfite, 564
sodium tartrate, 566
sodium thiosulfate, 568
stannate, 556
stannous chloride, 522
strontium sulfate, 558
succinate, 691
sulfate, 31, 45, 64, 121, 149, 1 66, 179,
220, 259, 274, 365, 378, 388, 397,
405, 480, 509, 512, 522, 526, 529,
530, 534, 541, 544, 552, 556-62,
643, 668, 719
sulfide, 564
sulfoantimonate, 500-1
sulfonates, 564
tantalum fluoride, 710
tartrate, 564-566
tellurate, 566
telluric acid oxalate, 552
tellurium bromide, 712
tetroxalate, 552
thiocyanate, 70, 566-7
thiosulfate, 568
titanium fluoride, 568
thorium sulfate, 724
tungstate, 530, 541, 562
uranyl butyrate, 733
uranyl carbonate, 512
uranyl chloride, 734
uranyl nitrate, 735
uranyl oxalate, 735
uranyl propionate, 736
uranyl sulfate, 736
vanadate, 568
yttrium oxalate, 747
zinc cyanide, 532
zinc sulfate, 557
zinc vanadate, 568
Praseodymium chloride, 568
dimethyl phosphate, 569
double nitrates, 568
glycolate, 568
molybdate, 568
Praseodymium chloride, oxalate, 568
sulfate, 569
sulfonates, 569
tungstate, 569
Probnal, 742
Propione, 300
Propiolic acid, phenyl, 570
Propionic acid, 303, 315, 436, 569-70
acid, amino, 19
acid, iodo, 570
acid, phenyl, 570
aldehyde, 570
Propionitrile, 571
Propyl acetate, 12, 571
alcohol, 5, 128, 511, 571-2, 574, 636,
647
alcohol, iso, 533
ammonium iodine, tetra, 54, 55
. ammonium perchlorates, 44
amine hydrochloride, 573
amines, 572-3
anisole, 73
benzene, 91
bromide, 293, 573
butyrate, 571
chloride, 573
Propylene, 573
Propyl formate, 571
iodide, 573
malonic acid, 399
piperidine, 262, 496
propionate, 571
sulfine perchlorate, 698
Pseudo cumidine, 279
Pyrene, 573
Pyridinamino succinic acids, 575
Pyridine, 21, 127, 136, 258, 279, 439,
446, 484, 486, 574
Pyridines, methyl, ethyl, etc., 574
trimethyl, 262
Pyrocatechol, 15, 77, 146, 224, 251,
324, 446, 575
Pyrogallol, 15, 224, 575
Pyrone, dimethyl (see Dimethylpy-
rone
Pyrophosphoric acid, 490
Pyrotartaric acid, 307, 711-2
Pyroxylin, 465
Buinaldine, benzoyl tetrahydro, 146
uinidine, 251, 575
salts, 575
sulfate, 576
Quinine, 128, 251, 576, 577
glycerophosphate, 578
hydrochloride, 578
pyrotartrates, 579
salicylate, 578
salts, 577-8
sulfate, 578
tannates, 579
Buinhydrone, 575
uinol, 132, 448
837
SUBJECT INDEX
Quinoline, 484, 486
ethiodide, 579
Radium emanations, 579^80
Rape oil, 468
Raffinose, 695-97
Resorcinol, 15, 77, 131, 146, 224,
283, 324, 446, 484, 495,
580-1, 654
Retene, 145
Rhamnitol, dibenzal, 698
Rhamnose, 696
Rhodium salts, 581
sodium nitrite, 660
Rosolic acid, 582
Rosaniline, 581
hydrochloride, 582
Rubidium alum, 32, 582
bicarbonate, 582
bromide, 582
bromiodide, 585
cadmium bromide, 168
cadmium chloride, 172
caesium nitrosochloride, 587
calcium sulfate, 218
carbonate, 582
chlorate, 583
chloride, 183, 270, 356, 371, 412
chromate, 584
cobalt nitrite, 259
dichromate, 584
dihydroxy tartrate, 587
double sulfates, 587
fluoboride, 582
fluoride, 27, 584
fluosilicate, 586
hydroxide, 536, 584-5
gold chloride, 308
iodate, 585
iodide, 585
iridate, 585
mercuric chloride, 412
molybdate, 585
nitrate, 586
perchlorate, 583
periodate, 585
periodides, 585
permanganate, 554, 586
platinum chloride, 498
potassium perchlorate, 583
ruthenium nitrosochloride, 587
selenate, 586
silicotungstate, 586
sulfate, 220, 587
tellurate, 586
telluric acid oxalate, 586
tellurium bromide, 712
tellurium chloride, 584, 712
thallium chloride, 583.
thiocyanate, 567
uranyl chloride, 734
uranyl nitrate, 735
Ruthenium salts, 587
251,
575,
Saccharin, 587-8
Salicin, 588
Salicylamide, 588
Salicylates, methyl and phenyl, 251
Salicylic acid, 15,, 136, 251, 480, 575,
588-93
aldehyde, 10
Salol, 9, 96, 149, 224, 225, 245, 309, 431,
448, 593
chl
Samarium chloride, 594
dimethyl phosphate, 594
double nitrates, 594
glycolate, 594
oxalate, 594
sodium sulfate, 594
sulfate, 594
sulfonates, 595
Santonin, 593
Scandium oxalate, 595
sulfate, 595
Schonite, 641
Scopolamine hydrobromide, 325
Sebacic acid, 595
Selenic acid, 596
Selenious acid, 597
anhydride, 597
Selenium, 334, 408, 421, 596, 720
583 bromide, diphenyl, 596
dioxide, 597
Silica, 210, 362, 378, 395, 402, 556, 597
Silicon, 598
iodides, 598
tetraphenyl, 302, 362, 598, 729
Silicotungstic acid, 598
Silver, 598, 705, 712
acetate, 598-9, 622
acetyl propionate, 617
arsenate, 600
arsenite, 600
benzoate, 600
borate, 600
bromate, 60 1
bromide, 351, 367, 507, 582, 601-4
butyrate, 604
caproates, 605
carbonate, 605
chloroacetate, 599-600
chlorate, 605
chloride, 183, 198, 270, 356, 371, 388,
583, 604-12
chromate, 612
citrate, 613
eyanide, 531, 613
dichromate, 613
ethyl methyl acetate, 600
ferricyanide, 613
fluoride, 613-4
fulminate, 614
heptoate, 614
iodate, 614-5
iodide, 271, 359, 374, 537, 604, 605,
611, 615-6
isobutyrate, 604
838
SUBJECT INDEX
Silver, isovalerate, 624
laurate, 617
levulinate, 617
malate, 617
methyl ethyl acetate, 600
myristate, 617
nitrate, 57, 546, 548, 599, 617-9
nitrite, 1 18, 209, 376, 549, 619-20, 660
onanthylate, 614
oxalate, 620
oxide, 620-1
palmitate, 617
permanganate, 621
phosphate, 621
propionate, 621
propyl (di) acetate, 600
salicylate, 621
selenides, 95, 152
sodium cyanide, 613
stearate, 617
succinate, 621
sulfate, 219, 378, 562, 621-3
sulfide, 29, 95, 101, 277, 365, 611, 624
sulfonates, 624
tartrate, 624
thallium cyanide, 613
thiocyanate, 567, 605, 624
valerates, 624-5
vanadate, 625
Sodammonium, 625
Sodium, 37, 625
acetate, 500, 626-7
acid phosphate, 663
alum, 32
ammonium phosphates, 62
ammonium sulfate, 68
ammonium sulfite, 69
antimony sulfide, 627-8
arsenates, 628-9
benzoate, 187, 629
beryllium fluoride, 148
biborate, 630-1
bicarbonate, 43, 634, 637-8
bisulfate, 670, 672
borate, 367
borate (tetra), 629-31
bromate, 631
bromide, 99, 167, 604-5, 631-2, 634-5
cacodylate, 633
cadmium bromide, 169
cadmium chloride, 174
cadmium iodide, 178
cadmium sulfate, 180
caesium sulfate, 186
calcium thiosulfate, 222
camphorates, 633
carbonate, 13, 218, 509, 512, 633-7,
647, 655
cerium sulfate, 243
chlorate, 639
chloride, 45, 49, 109-11, 121, 166,
170, 174, 183, 196-8, 267-8, 270,
274, 339, 356, 371, 388, 411, 48o,
507, 512, 517, 519, 521-2, 526,
544-5, 548, 562, 583, 611, 632, 635,
637, 639-49, 66 1, 669-71, 690
chromates, 649-52
cinnamate, 652
citrate, 652
copper sulfate, 276
cyanide, 270, 531, 613, 649
dichromate, 650-2
diethyl barbiturate, 629
dihydrogen phosphate, 663
ferrocyanide, 532, 652
fluoride, 27, 175, 357, 534, 632, 649,
652
fluosilicate, 652 •
fluozirconate, 676
formate, 653
gadolinium sulfate, 305
glycerophosphate, 653
gold chloride, 308
hydrogen arsenate, 629
hydrogen phosphate, 662
hydrosulfite, 673
hydroxide, 109, 113, 536, 585, 627,
629, 630, 632, 643, 649, 651-4,
663, 670
iodate, 654
iodide, 177, 616, 632, 634, 649, 652,
654-6
iodide mercuric cyanide, 423
iodomercurate, 656
iron sulfate, 344
lanthanum sulfate, 348
lithium sulfate, 377
lithium tartrate, 378
magnesium sulfate, 668
manganese sulfate, 404
mercuric chloride, 41 1
mercury iodide, 656
meta borate, 502, 631
meta phosphate, 631
meta vanadate, 676
molybdate, 440, 656
nickel sulfate, 454
nitrate, 55, 58, 109, 116-7, 208, 222,
360, 376, 509, 519, 545-6, 548, 618,
632, 635, 644-5, 656-61
nitrite, 649, 659-60
nitrophenol, 662
oleate, 480, 660
oxalate, 552, 660-1
palmitate, 661
perchlorate, 639
phenolate, 662
phenol sulfonate, 674
phosphate, 662
phosphate fluoride, 664
phosphites, 664
picrate, 664
potassium carbonate, 512
potassium sulfate, 559, 668
potassium tartrate, 566
potassium thiosulfate, 568
839
SUBJECT INDEX
Sodium, pyrophosphate, 631, 649, 664
rhodonitrite, 660
salicylate, 187, 590, 665
samarium sulfate, 594
selenate, 665
silicate, 119, 213, 378, 396, 631, 665
silver cyanide, 613
stannate, 665
succinates, 665-6
sulfate, 121, 179, 218, 220, 259-60,
274, 365, 378, 397, 405, 522, 526,
559, 562, 623, 632, 637, 641, 649,
651-2, 656, 658, 660-1, 667-72,
747
sulfide, 455, 672
sulfite, 673
sulfoantimonate, 627-8
sulfonates, 673-4
tartrate, 566, 674
tellurates, 674
tetraborate, 367, 629-31
tetrachromate, 650
tetraiodofluorescein, 335
thiocyanate, 567
thiosulfate, 208, 222, 628, 674-5
thorium sulfate, 725
trichromate, 650
tungstate, 656, 665, 672, 675
uranyl chromate, 734
uranyl oxalates, 66 1
urate, 676
yttrium sulfate, 747
zinc sulfate, 755
zirconium fluoride, 676
Sorbitols, benzal, 698
Sorbose, 697
Sparteine, 676
sulfate, 676
Stannous, stannic (see Tin)
Stearic acid, 97, 248, 446, 467-8, 475,
676-7
Stearin, tri, 225, 467, 475, 677
Stilbene, 88, 103, 123, 133, 147, 280,
677
Strontium acetate, 677
ammonium sulfate, 68
benzoate, 678
bromate, 678
bromide, 100, 678
camphorate, 678
carbonate, 649, 678-9
chlorate, 679
chloride, 100, in, 119, 170, 198,
356, 371, 388, 526, 649, 679, 680
chromate, 680
cinnamate, 68 1
fluoride, 680, 68 1
formate, 68 1
glycerophosphate, 68 1
hydroxide, 678, 680-2
hyposulfate, 365
iodate, 682
iodide, 682
Strontium acetate, iodide mercuric cy-
anide, 423
iodomercurate, 682
malate, 683
malonate, 683
mercuric, iodide, 682
molybdate, 683
nitrate, 361, 546, 548, 659, 68 1, 683
nitrite, 620, 683-4
oxalate, 684
oxide, 157, 198, 680, 684
periodide, 682
permanganate, 684
potassium sulfate, 558
salicylate, 684
silicate, 378, 665
succinate, 685
sulfate, 378, 562, 672, 680, 685-6
tartrate, 686
tungstate (di), 686
Strychnine, 687
salts, 688-9
Suberic acid, 689
Succinic acid, 136, 480, 666, 690-2
acid, amino, 692
acid, bromo, 692
acid, chloro, 692
acids, pyridinamino, 575
acid nitrile, 102, 133, 135, 224, 299,
405,445, 618, 649,693
Succinimide, 693
Sucrose (see Sugar)
Sugar, 166, 187, 198, 205, 397, 512,
548, 627, 636, 648, 672, 693-8
Sulfanilic acid, 698
Sulfine chloroplatinates, 499
Sulfonal, 435, 448, 593
Sulfonium perchlorates, 698
iodide, triethyl, 699
Sulfur, 76, 127, 130, 150, 160, 247,
334, 421, 446, 489, 564, 596, 672,
699-705, 720, 729
dioxide, 160, 224, 247, 315, 436, 438,
705-8
Sulfuric acid, 5, 9, 10, 16, 124, 136,
145, 146, 278, 279, 484, 486, 575,
708-9, 726, 731
Sulfon methanes, ethyl, and methyl, 435
Sulfur trioxide, 708-9
Sulfuryl chloride, 247, 708
"Superphosphates," 212
Syngenite, 218
Tachhydrite, 196, 641
Talitol, tribenzal, 698
Tannic acid, 710
Tantalum potassium fluoride, 710
Tartaric acid, 480, 481, 710-11
Telluric acid, 712
Telluric acid caesium oxalate, 185
acid potassium oxalate, 552
acid rubidium oxalate, 586
Tellurium, 334, 596, 705, 712, 720
840
SUBJECT INDEX
Tellurium, bromide, diphenyl, 596
caesium chloride, 182
chromium alum, 249
double salts, 712
rubidium chloride, 584
tetra iodide, 713
Terephthalic acid, 490
Terpin hydrate, 712
Tetra hydrobenzene, 89
iodo pyrrol, 335
Tetronal, 435
Thallium alum, 32, 713
bisulfate, 720
bromate, 713, 716
bromide, 713
caesium chloride, 182
carbonate, 713
chloride, in, 150, 170, 183, 198, 270,
339, 356, 371, 388, 526, 583, 611,
649, 680, 713, 715-8
chlorate, 714
chromate, 717
cyanide, 717
double cyanides, 717
double sulfates, 720
fluoride, 717
hydroxide, 717
iodate, 718
iodide, 713, 718
mercuric cyanide, 423
nitrate, 547, 548, 619, 659, 718
oxalate, 718
perchlorate, 714
phosphate, 718
picrate, 719
platinum chloride, 498
rubidium chloride, 584
selenate, 719
silver cyanide, 613
sulfate, 31, 719-20
sulfide, 720
sulfite, 720
thiocyanate, 716, 720
vanadates, 721
Thallo thallic chloride, 717
Thebaine, 721
Theobromine, 187, 721
Theocin, 721
Theophylline, 721
Thiocarbamide (thiourea), 70
diodo di, 226
Thiophene, 128
carbonic acids, 721
Thiophenylazine, 123
Thiosinamine, 738
Thiourea (thiocarbamide), 70, 738
Thorium ammonium oxalate, 60, 722
ammonium sulfate, 724
borate, 722
chloro acetates, 721
chloro oxalate, 723
emanations, 721
hippurate, 722
Thorium ammonium oxalate, nitroben-
zene sulfonate, 725
oxalate, 722-3
picrate, 723
potassium sulfate, 724
selenate, 723
sodium sulfate, 725
sulfate, 723-5
Thoulet solution, 541
Thulium bromo nitrobenzene sulfo-
nate, 725
oxalate, 725
Thymol, 5, 10, 146, 227, 251, 446, 484,
495, 593, 725-6
Tin, 334, 705, 712, 726
chloride, 170, 198, 247, 270, 356, 371,
388, 401, 522, 713, 726-7
diphenyl, 430
hydroxide, 728
iodide, 728-9
oxalate, 729
potassium chloride (ous), 522
sulfate, 729
sulfide (ous), 95
tetraphenyl, 598, 729
triphenyl, 95
Titanium potassium fluoride, 568
silicate, 119
Tolane, 103, 123, 147
Toluene, 21, 87, 88, 93, 239, 247, 278,
293, 301, 313, 481, 704, 729-30,
745
bromo, 128, 227, 293, 301, 484, 572,
693, 726, 730
chloro, 87, 93
chloro nitro, 730
dinitro, I
nitro, 24, 26, 27, 77, 79, 87, 93, 128,
132, 283, 293, 300, 303, 408, 421,
446, 465, 478, 729-30
sulfonamines, 729
sulfochloride, 730
trinitro, I, 16, 224, 495, 575
Toluic acids, 9, 10, 12, 136, 575, 730,
731
Toluidines, 79, 136, 224, 240, 283, 293,
324, 431, 446, 448, 484, 486, 581,
731-2
Tolyl carbamide, 226
Trehalose, 696
Tribenzylamine, 730
Triethylamine, 102, in (see Ethyl-
amine)
Trimethylamine, 437 (see Methyl-
amines)
Trimethylethylene, 72
Triolein, 467
Trional, 435
Trioxymethylene, 303
Tripalmitin, 467, 475
Triphenylamine, 282, 732
Triphenyl arsine, 732
Triphenylbismuthine, 732
841
SUBJECT INDEX
Triphenyl phosphine, 732
guanidine, 2
stibene, 732
Tristearin, 467, 475, 677
Trithioacetaldehyde, 732
Trithiobenzaldehyde, 732
Tropaeolin, 309
Tropic acid, 732
Tungsten trioxide, 675
Turpentine, 294, 440, 733
Ulexine, 280
Uranyl ammonium carbonate, 43, 733-4
ammonium oxalate, 735
ammonium propionate, 736
caesium chloride, 734
chloride, 733-4
double nitrates, 735
iodate, 734
nitrate, 734-5
oxalate, 66 1, 735-6
potassium butyrate, 733
potassium carbonate, 512
potassium chloride, 734
potassium oxalate, 735
potassium propionate, 736
potassium sulfate, 736
rubidium chloride, 734
sodium chromate, 734
sodium oxalates, 66 1
sulfate, 736
tetra methyl ammonium chloride, 734
Uranium sulfate, 736
Urea, 279, 484, 486, 737-8
diphenyl, 738
Urethan, 80, 128, 283, 296, 421, 446,
484. 593, 730, 741-2
derivatives, 742
methyl, 431
Uric acid, 742-3
Ureide of glucose, 741
Valeramides, 744
Valeric acid, 743
Vanadium ammonium sulfate, 69
caesium alum, 180
rubidium alum, 582
thallium alum, 713
Vanillic aldehyde, 2
Vanillin, 9, 10, 744
Vaselin, 5
Veratrine, 744
Veratrol, 730, 744
Veronal, 742, 744
Vesuvin, 744
Vinyl sulfine perchlorate, 698
Water, 5, 125, 131, 133, 138-42, 144,
164-6, 227, 235, 245, 248, 280,
282, 285, 287, 294-5, 297, 299,
302, 468, 487, 589, 593, 729, 730,
Weldmint oil, 468
Xanthine, dimethyl, 721
Xanthone, 132
Xenon, 745
Xylenes, 2, 5, 21, 88, 94, 128, 281, 294,
301, 484, 581, 693, 705, 730, 744
nitro, 745
Xylenol, 745
Xylidene, 79, 484
Xylitol, dibenzal, 698
Xylose, 696
Ytterbium benzene sulfonate, 746
cobalticyanide, 746
dimethyl phosphate, 746
oxalate, 746
sulfate, 746
Yttrium chloride, 746
cobalticyanide, 746
dimethyl phosphate, 747
glycolate, 746
hydroxide, 747
iodate, 746
malonate, 746
nitrate, 747
oxalate, 747
potassium oxalate, 747
sodium sulfate, 747
sulfate, 747
sulfonates, 748
tartrate, 748
Zein, 748
Zinc, 150, 712
acetate, 748
ammonium chloride, 751
ammonium oxalate, 754
ammonium phosphate, 754
ammonium sulfate, 69, 273
arsenite, 748
benzoate, 749
bicarbonate, 749
bismuth nitrate, 151
bromide, 749
caesium sulfate, 186
carbonate, 749
cerium nitrate, 242
chlorate, 750
chloride, in, 150, 170, 198, 270,
339, 356, 388, 401, 680, 713, 727,
750-1
chromates, 751
cinnamate, 752
cyanide, 531, 752
fluoride, 652, 752
gadolinium nitrate, 304
hydroxide, 752-3
iodate, 753
iodide, 753
lanthanium nitrate, 347
mercuric thiocyanate, 752
neodymium nitrate, 449
nitrate, 395, 754
oxalate, 60, 754
842
SUBJECT INDEX
Sine, oxychlorides, 750 Zinc, sulfate, 274-5, 404. 754~5
phenol sulfonate, 756 sulfide, 277, 345, 365, 624, 755
potassium cyanide, 532 sulfite, 755
potassium sulfate, 557 sulfonates, 755-6
potassium vanadate, 568 tartrate, 756
praseodymium nitrate, 568 thallium cyanide, 717
rubidium sulfate, 587 thallium sulfate, 720
samarium nitrate, 594 valerate, 756
silicate, 178, 378 Zirconium sodium fluoride, 676
sodium sulfate, 755 sulfate, 756
843
Table Showing the Volume Number and Corresponding Year
(Those journals marked (*) were examined page by page for solubility data. In
last number recorded for each journal is that
1900
1901
1902
1903
1904
IQ05
1906
Am Chem Jour. (*)
23-4
72
W9-io
25
310-14
l7llQ-2I
W?-3
238
1%
33
25-6
73
1 1-2
26
314-19
22-24
6
4-6
239
10
34
27-8
74
13-4
27
320-26
25-27
7
7-9
240
n
35
29-30
75
15-6
28
326-30
28-30
8
IO-I2
241
12
36
3J~2
76
17-8
29
«rf
9
13-15
242
13
37
33-4
77
19-20
30
338-43
4-6
10
16-18
243
14
38
35-6
78
21-2
31
344-51
7-9
ii
19-21
244
15
39
i
35
20
Am Jour Pharm. (*)
Am. Jour. Sci. (t)
Analyst (t)
Ann Chem (Liebig's) (t)
Ann chim phys.* (*)
Ann chim anal, (t) ". • •
Ann. Physik (Wied.) (t)
Arch. Pharm. (f) -
Atti accad Lincei (*)
Ber (*)
Biochem, J. (t)
Bull soc chim (*)
l3]23
14
25
IS
27
16
29
17
i
33
19
Bull. soc. chim. belg. (*)
Chem. Abs. (*)
Chem. News (t) . . .
81-2
83-4
85-6
87-8
89-90
I
28
138-9
IO-II
34
91-2
2
29
I4O-I
11-12
35
93-4
3
30
142-3
12-13
36
6th
28
1-2
89
4
Chem. Weekblad (*)
Chem. Ztg
24
130-1
6-7
30
4th
22
25
132-3
7-8
3i
23
26
134-5
8-9
32
24
27
136-7
9~IO
53ti
25
Compt. rend, (f)
Elektrochem Z (f)
Gazz chim ital (*)
Intern. Congr. Appl. Chem. (t)
J Am Chem. Soc (*) . .
26
27
i
87
3
J Biol. Chem. (t)
J. Chem. Soc. (Lond.) (*) . .
77
79
81
83
i
85
2
T. chim. Dhvs. (*) .
J. Ind. Eng. Chem. (*) . .
J. pharm. chim. (t)
J. Phys. Chem. (*)
I6hl-12
big '
W6I-2
32
19
21
64-5
i3~I4
5
10
63-4
33
20
22
66-7
15-16
6
Mr
65-6
34
21
68-9
17-18
7
2
67-8
35
22
I. .
I9-2O
8
3
69-70
36
23
21-22
9
4
71-2
37
24
23-24
10
5
73-4
38
25
J. physique (f)
J. prakt. Chem. (t)
J. Russ. Phys. Chem. Soc
J. Soc. Chem. Ind. (f)
Mem. Coll. Sci. Eng. Kyoto2 (*)
Monatsh. Chem. (f)
24
7O-I
'5:6
16-17
5-6
24-25
71-2
22
3-4
42
16
33-37
9
37
42-46
37-40
25
72-3
'7-8
18-19
6-7
25
73-5
23
5-6
43
17
38-42
10
38-9
47-50
40-43
26
74-5
9-10
2O-2I
7-8
25-26
76(A)
24
7-8
44
18
43-48
ii
40
50-54
43-46
27
76-7
i
11-12
22-23
8-9
26-27
77-8(A)
25
9-10
45
19
48-51
12
41-2
54-57
47-50
Pharm. Jour. (Lond.) (*)...
Philippine J Sci (A) (t)
Phil. Mag. (f) .
151SO
IO-II
2
23
66-7
iQ
Wl-2
12-13
3
23-24
68-9
20
3-4
14-15
4
24
69-71
21
1-2
41
IS
29-33
8
35-6
39-42
34-7
Phys. Rev. (t) . . . .
Proc. k. Akad. Wet. (Amst.) (*)
Proc. Roy. Soc. Edinburgh (f) .
Proc. Roy. Soc. (Lond.) (f) . . .
Rec. trav. chim. (*)
Trans. Am. Electrochem. Soc.(f)
Z. anal. Chem. (*) . .
39
13
22-25
6-7
33
32-35
30-1
40
14
26-29
7
34
36-39
3i-4
Z. angew. Chem. (f)
Z. anorg. Chem. (*)
Z. Elektrochem. (*)
Z. Kryst. Min.
Z. physik. Chem. (*)
Z physiol Chem (f)
1 Changed to Ann. chim. in 1914.
Changed to Mem. Coll. Sci. (Kyoto) in 1914.
of Publication of Fifty Chemical and Related Periodicals.
the case of those marked (f), the tables of contents only were searched. The
of the last complete volume examined.)
1907
1908
1909
1910
1911
1912
1913
1914
I9I5
1916
1917
37-8
39-40
41-2
43-4
45-6
47-8
49-50
79
80
81
82
83
84
85
"86"
'87'
'ss'
89'
23~4
25-26
27-8
29-30
31-2
33-4
35-6
37-8
39-40
41-2
43-
32
33
34
35
36
37
38
39
40
351-58
358-64
364-71
371-78
378-86
386-94
395-402
402-4
IO-I2
13—15
16-18
19-21
22-24
25-27
28-30
1-2
3-4
12
j?
J4
15
16
17
18
19
20
22-24
25-27
28-30
34-36
37-40
40-43
43-46
46-48
48-
245
246
247
248
249
250
251
252
253
16
I7
18
19
20
21
22
23
24
25
40
42
43
44
45
46
47
48
2
3
4
5
5
6
7
8
9
10
Ml
3
5
7
9
ii
13
15
17
19
2 T
22
24.
2?
26
27
i
2
3
T"
4
o
5
6
7
8
9
IO
ii
95-6
97-8
99-100
IOI-2
103-4
105-6
107-8
109-10
III-I2
"3-14
4
5
6
7
8
9
IO
ii
12
13
14
31
144-5
32
146-7
33
148-9
34
150-1
35
152-3
36
154-5
37
156-7
158-9
39
160-1
162-3
14-15
15-16
16-17
17-18
18-19
19-20
20-21
21-22
22-
37
38
39
40
41
42
43
44
45
46
7th
8th
29
30
/ •**
31
32
33
34
35
36
37
38
39
2-3
4-5
5-7
7-8
11-13
13-16
16-19
20-23
24-28
28-32
91
93
95
97
99
IOI
103
105
107
109
in
5
6
7
8
9
IO
ii
12
13
14
i
2
3
4
5
6
7
8
9
25-26
27-28
29-30
3-4
5-6
7-8
9-10
11-12
ii
12
13
14
IS
16
17
18
19
20
21
6
7
8
9
[sir
2
3
4
75-6
77-8
79-80
81-2
83-4
85-7
87-9
89-90
91-2
39
40
42
43
44
45
46
47
26
27
28
29
30
31
32
33
34
35
36
1-2
2-3
3-4
4~5
5 [new series Vol. ii
28
29
3°
31
32
34
35
36
78-9
80-1
82-3
84-5
86-7
88-9
90-1
92-3
94-5
2
3
4
5
6
7
8
9
10
ii
12
13-14
15-16
17-18
19-20
21-2
24-25
26-27
28-29
30-31
32-33
34-35
Nl-2
3-4
5-6
7—
9-IO
10-11
11-12
12-13
14-15
15-16
16-17
17-
27-28
79(A)
28-29
8o-i(A)
29-30
82-3(A)
30-31
83-4(A)
84^6(A)
32-33
86-7(A)
88%(A)
34-
89-91 (A)
91-
26
27
28
29
30
31
32
33
34
11-12
15-16
17-18
19-20
21-22
23-24
25-26
27-28
29-30
31-
46
47
48
49
50
51
52
53
54
2O
21
22
23
24
25
26
27
28
52-56
56-60
61-65
65-69
69-73
73-79
79-84
84-90
90-93
14
15
16
17
18
19
20
21
42-4
44-5
46
47
48-9
50
51-2
53
57-61
61-65
65-68
68-75
75-78
78-81
8 1-86
86-89
89-90
50-54
55-58
59-64
64-70
70-76
77-82
83-88
89-93
93-95
D. VAN NOSTRAND COMPANY
25 PARK PLACE
NEW YORK
SHORT-TITLE CATALOG
OP
publications ana Jmjwrtatums
OF
SCIENTIFIC AND ENGINEERING
BOOKS
This list includes
the technical publications of the following English publishers:
SCOTT, GREENWOOD & CO. JAMES MUNRO & CO., Ltd.
CONSTABLE&COMPANY,Ltd. TECHNICAL PUBLISHING CO.
BENN BROTHERS, Ltd.
for whom D. Van Nostrand Company are American agents.
DECEMBER, lt)lij
SHORT-TITLE CATALOG
OF THE
Publications and Importations
OF
D. VAN NOSTRAND COMPANY
25 PARK PLACE, N. Y.
All Trices in this list are JVE,T.
bindings are in cloth unless otherwise noted.
Abbott, A, V, The Electrical Transmission of Energy 8vo, *$s oo
A Treatise on Fuel i5mo, o 75
Testing Machines i6mo, o 75
Abraham, Herbert. Asphalts and Allied Substances 8vo, 5 oo
Adam, P. Practical Bookbinding iirao, 2 50
Adams, H. Theory and Practice in Designing Svo, *2 50
Adams, H. C. Sewage- of Sea Coast Towns 3vo, *2 50
Adams, J. W. Sewers and Drains for Populous Districts 8vo, 2 50
Addyman, F. T. Practical X-Ray Work 8vo, 5 oo
Adler, A. A. Theory of Engineering Drawing 8vo, 2 50
— Principles of Parallel Projecting-line Drawing Svo, i 25
Aikman, C. M. Manures and the Principles of Manuring 8vo,
(Reprinting.)
Aitken, W. Manual of the Telephone 8vo, *8 oo
d'Albe, E. E. F. Contemporary Chemistry i2mo, i 50
Alexander, J. Colloid Chemistry lamo, i oo
Allan, W. Strength of Beams Under Transverse Loads i6mo, 075
Theory of Arches i6mo,
Allen, H. Modern Power Gas Producer Practice and Applications. 12010,
(Reprinting.)
Anderson, J. W. Prospector's Handbook izmo, i 75
Andes, L. Vegetable Fats and Oils 3vo, *6 oo
— Animal Fats andi Oils Svo, 5 oo
- Drying Oils, Boiled Oil, and Solid and Liquid Driers Svo, *6 oo
— Iron Corrosion, Anti-fouling and Anti-corrosive Paints Svo, <5 oo
— Oil Colors, and Printers' Ink Svo, 4 oo
— Treatment of Paper for Special Purposes i2rao, 3 oo
Andrews, E. S. Reinforced Concrete Construction iamo, *2 oo
- Theory and Design of Structures Svo, *3 50
Further Problems in the Theory and Design of Structures. .. .8vo, *2 50
— The Strength of Materials .8vo, *4 oo
— Elastic Stresses in Structures Svo, 9 oo
Andrews, E. S., and Hey wood, H. B. The Calculus for Engineers. i2mo, *2 oo
Annual Reports on the Progess of Chemistry. Fifteen Volumes now
ready. Vol. I., 1904, Vol. XV., 1919 Svo, each, 2 oo
Argand, M. Imaginary Quantities , i6mo, o 75
Armstrong, R., and Idell, F. E. Chimneys for Furnaces and Steam Boilers.
o 75
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 3
Arnold, E. Armature Windings of Direct-Current Dynamos 8vo, 2 oo-
Asch, W., and Asch, D. The Silicates in Chemistry and Commerce . Svo, 7 50
Ashe, S. W., and Keiley, J. D. Electric Railways. Theoretically and
Practically Treated. Vol. I. Rolling Stock i2mo, *2 50
Ashe, S. W. Electric Railways. Vol. II. Engineering Preliminaries and
Direct Current Sub-Stations i2mo, *2 50
Electricity: Experimentally and Practically Applied i2mo, *2 oo
Ashley, R. H. Chemical Calculations i2mo, 2 50
Atkins, W. Common Battery Telephony Simplified i2mo, *i 25
Atkinson, A. A. Electrical and Magnetic Calculations 8vo, *i 50-
Atkinson, J. J. Friction of Air in Mines i6mo, o 75.
Atkinson, J. J., and Williams, Jr., E. H. Gases Met with in Coal Mines.
i6mo, o 75
Atkinson, P. The Elements of Electric Lighting i2mo, i 50
The Elements of Dynamic Electricity and Magnetism i2mo, 2 oo
Auchincloss, W. S. Link and Valve Motions Simplified 8vo, *i 50
Audley, J. A. Silica and the Silicates 8vo (In Press.)
Austin, E. Single Phase Electric Railways -4*0, *s oo
Austin and Cohn. Pocketbook of Radiotelegraphy (In Press.}
Ayrton, H. The Electric Arc 8vo, 5 50
Baff, W. E. Sale of Inventions i2mo (In Press.)
Bailey, R. D. The Brewers' Analyst Svo, *5 oo
Baker, A. L. Quaternions Svo, i 50
Thick-Lens Optics i2mo, *i 50
Baker, Benj. Pressure of Earthwork i6mo,
Baker, G. S. Ship Form, Resistance and Screw Propulsion Svo, *4 50
Baker, I. 0. Levelling i6mo, o 75
Baker, M. N. Potable Water . . i6mo, o 75
Sewerage and Sewage Purification i6mo, o 75
Baker, T. T. Telegraphic Transmission of Photographs i2mo,
(Reprinting.)
Bale, G. R. Modern Iron Foundry Practice. i2mo.
Vol. I. Foundry Equipment, Materials Used..... *3 oo>
Ball, J. W. Concrete Structures in Railways Svo, *2 50-
Ball, R. S. Popular Guide to the Heavens Svo, *5 oo
Natural Sources of Power Svo, 2 50
Ball, W. V. Law Affecting Engineers: Svo, *3 50
Bankson, Lloyd. Slide Valve Diagrams i6mo, o 75
Barham, G. B. Development of the Incandescent Electric Lamp.. Svo, 2 50
Barker, A. F. Textiles and Their Manufacture Svo, 2 50
Barker, A. F., and Midgley, E. Analysis cf Woven Fabrics Svo, 3 50
Barker, A. H. Graphic Methods of Engine Design i2ino, 2 oo
— - Heating and Ventilation 4to, 9 oo
Barnard, J. H. The Naval Militiaman's Guide i6mo, leather i oa
Barnard, Major J. G. Rotary Motion i6mo, o 75
Barnes, J. B. Elements of Military Sketching i6mo. *o 75
Barnett, E. deB. Coal-Tar Dyes and Intermediates Svo, 3 50-
Explosives, Matches and Pyrotechny .Svo (In Press.)
Synthetic Dyes Svo (In Press.)
Barrowoliff, M., and Carr, F. H. Organic Medicinal Chemicals. .Svo,
(In Press.)
4 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Barrus, G. H. Engine Tests 8vo, *4 oo
Baterden, J. R. Timber 6\o, *2 50
Bates, E. L., and Charlesworth, F. Practical Mathematics and
Geometry lamo,
Part I. Preliminary Course i oo
Part II. Elementary Course i oo
Part HI. Advanced Course i 50
— Practical Mathematics lamo, *2 oo
— Practical Geometry and Graphics i2mo, 2 oo
Batey, J. The Science of Works Management i2mo, *2 oo
— Steam Boilers and Combustion i2mo, *2 oo
Bayonet Training Manual i6mo, o 30
Beadle, C. Chapters on Papermaking. Five Volumes i2mo, each, *2 oo
Beaumont, R. Color in Woven Design 8vo, *6 oo
— Finishing of Textile Fabrics 8vo, *s oo
— Standard Cloths 8vo, *6 oo
Beaumont, W. W. The Steam-Engine Indicator 8vo, 2 50
Bechhold, H< Colloids in Biology and Medicine 8vo, 5 oo
Beckwith, A. Pottery 8vo, paper, o 60
Bedell, F. Airplane Characteristics 8vo, i 60
— The Air Propeller 8vo, i oo
— The Airplane 8vo (In Press.)
Bedell, F., and Pierce, C. A. Direct and Alternating Current Manual.
8vo, 2 oo
Beech, F. Dyeing of Cotton Fabrics 8vo, 5 oo
— Dyeing of Woolen Fabrics 8vo, *s 50
Beggs, G. E. Stresses in Railway Girders and Bridges (In Press.}
Begtrup, J. The Slide Valve 8vo, *2 oo
Bender, 'C. E. Continuous Bridges i6mo, o 75
—'Proportions of Pins Used in Bridges i6mo, o 75
Bengouga, G. D. Brass (In Press.)
Bennett, EL G. The Manufacture of Leather 8v», 6 oo
— Animal Proteids 8vo, (In Press.)
^ernthsen, A. A Text-book of Organic Chemistry i2mo, 3 5°
;Bersch, J. Manufacture of Mineral and Lake Pigments 8vo, 6 oo
Be^eridge, J. Papermaker's Pocket Book i2mo, *4 ou
Binnie, Sir A. Rainfall Reservoirs and Water Supply 8vo, 4 oo
Binns, C. F. Manual of Practical Potting 8vo, 8 oo
- The Potter's Craft ; i2mo> *2 oo
Birchmore. W. H. Interpretation of Gas Analysis i2mo, *i 25
Blaine, R. G. The Calculus and Its Applications ismo, *i 75
Blake, W. H. Brewers' Vade Mecum 8vt>, *4 oo
Blanchard, W. M. Laboratory Exercises in General Chemistry. . i2mo, i oo
; Blasdate, W. C. Quantitative Chemical Analysis i2mo, 2 50
Bloch, "L. Science of Illumination 8vo, 2 50
Blyth, A, W. Foods: Their Composition and Analysis 8vo, 8 5*
— Poisons: Their Effects and Detection 8vo, 8 50
Bikkmaam, F. Celluloid i2mo, *2 50
Bodmer, G. R. Hydraulic Motors and Turbines i2mo, 5 oo
Boileau, J. T. Traverse Tables 8vo, 5 oo
Bonney, G. E. The Electro-platers' Handbook i2mo, i 50
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 5
Booth, N. Guide to the Ring-spinning Frame i2mo, *2 oo
Booth, W. H. Water Softening and Treatment 8vo (Reprinting.)
— Superheaters and Superheating and Their Control 8vo, *i 50
Bottcher, A. Cranes: Their Construction, Mechanical Equipment and
Working 4to (Reprinting.)
Bottler, M. Modern Bleaching Agents zamo, 2 50
Bottone, S. R. Magnetos for Automobilists i2mo, *i oo
— Electro-Motors, How Made and How Use lamo, i oo
Boulton, S. B. Preservation of Timber i6mo, o 75
Bourcart, E. Insecticides, Fungicides and Weedkillers 8vo, *6 oo
Bourgougnon, A. Physical Problems. i6mo, o 75
Bourry, E. Treatise on Ceramic Industries 8vo, 6 oo
Bowie, A. J., Jr. A Practical Treatise on Hydraulic Mining 8vo, 5 oo
Bowls, 6. Tables of Common Rocks i6mo, o 75
Bowser, E. A. Elementary Treatise on Analytic Geometry i2mo, i 75
Elementary Treatise on the Differential and Integral Calculus . 12 mo, 2 25
— - Elementary Treatise on Analytic Mechanics i2mo, 3 oo
— — Elementary Treatise on Hydro-mechanics i2mo, 2 50
A Treatise on Roofs and Bridges i2mo, *2 25
Boycott, G. W. M. Compressed Air Work and Diving 8vo, *4 25
Bradford, G, Whys and Wherefores of Navigation i2mo, 2 oo
— Sea Terms and Phrases i2mo, fabrikoid (In Press. )
Bragg, E. M. Design of Marine Engines and Auxiliaries 8vo, 4 oo
Brainard, F. R. The Sextant i6mo,
Brassey's Naval Annual for 1919 8vo, 10 oo
Briggs, R., and Wolff, A. R. Steam-Heating i6mo, o 75
Bright, C. The Life Story of Sir Charles Tilsoji Bright 8vo, *4 50
— Telegraphy, Aeronautics and War 8vo, 6 oo
Brislee, T. J. Introduction to the Study of Fuel. .8vo (Reprinting.)
Broadfoot, S. K. Motors: Secondary Batteries i2mo, o 75
Broughton, H. H. Electric Cranes and Hoists
Brown, G-. Healthy Foundations i6mo, o 75
Brown, H. Irrigation 8vo (Reprinting.)
Brown, H. Rubber 8vo, 2} 50
W. A. Portland Cement Industry 8vo, 3 oo
Brown, Wm. N. Dipping, Burnishing, Lacquering and Bronzing
Brass Ware i2mo, *i 50
— Handbook on Japanning i2mo, *2 oo
Brown, Wm. N. The Art of Enamelling on Metal i2mo, *2 oo
— House Decorating and Painting i2ino, *2 oo
— History of Decorative Art i2mo *o 50
— Workshop Wrinkles 8vo, *i oo
Browne, C. L. Fitting and Erecting of Engines 8vo, *i 50
Browne, R. E. Water Meters i6mo, o 75
Bruce, E. M. Detection of Common Food Adulterants i2mo, i 40
Brunner, R. Manufacture of Lubricants, Shoe Polishes and Leather
Dressings 8vo, 3 50
Buel, R. H. Safety Valves iGmo, o 75
Bunkley, J. W. Military and Naval Recognition Book i6mo, i oc
Burley, G. W. Lathes. Their Construction and Operation 12010, 2 oo
— Machine and Fitting Shop Practice. 2 vols izmo, each, 2 oo
— Testing of Machine Tools i2mo, 2 oo
Burnside, W. Bridge Foundations i2mo, *2 oo
,6 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Burstall, F. W. Energy Diagram for Gas. With Text 8vo, i 50
Diagram. Sold separately *i oo
Burt, W. A. Key to the Solar Compass i6mo, leather, 2 50
Buskett, E. W. Fire Assaying i2mo, *i 25
Butler, H. J, Motor Bodies and Chassis . 8vo, *3 oa
Byers, H. G., and Knight, H. G. Notes on Qualitative Analysis. . . ,8vo,
(New Edition in Preparation.)
Cain, W. Brief Course io the Calculus i2mo, *i 75
Elastic Arches i6mo, o 75
. Maximum Stresses i6mo, o 75
Practical Designing Retaining of Walls i6mo, o 75
Theory of Steel-concrete Arches and of Vaulted Structures.
iGmo, o 75
Theory of Voussoir Arches i6mo, o 75
Symbolic Algebra i6mo, o 75
Calvert, G. T. The Manufacture of Sulphate of Ammonia and
Crude Ammonia i2mo, 4 oo
Camm, S.^ Aeroplane Construction xarno, 3 oo
Carhart, H. S. Thermo Electromotive Force in Electric Cells,
(In Press.}
Carey, A. E., and Oliver, F. W. Tidal Lands 8vo, 5 oo
Carpenter, F. D. Geographical Surveying i6mo,
Carpenter, R. C., and Diederichs, H. Internal Combustion Engines. 8vo, 5 50
Carter, H. A. Ramie (Rhea), China Grass i2mo, *3 oo
Carter, H. R. Modern Flax, Hemp, and Jute Spinning 8vo, *3 50
Bleaching, Dyeing and Finishing of Fabrics 8vo, *i 25
Cary, E. R. Solution of Railroad Problems with the Slide Rule. . i6mo, *i oo
Casler, M. D. Simplified Reinforced Concrete Mathematics i2mo, *i oo
Cathcart, W. L. Machine Design. Part I. Fastenings 8vo, *3 oo
Cathcart, W. L., and Chaff e e, J. I. Elements of Graphic Statics. . .8vo, *3 oo
• Short Course in Graphics i2mo, i 50
Caven, R; M., and Lander, G. D. Systematic Inorganic Chemistry. i2mo, 2 25
Chalkley, A. P. Diesel Engines 8vo, *4 oo
Chalmers, T. W. The Production and Treatment of Vegetable Oils,
4to, 7 50
Chambers' Mathematical Tables 8vo, 2 50
Chambers, G. F. Astronomy i6mo, *i 50
Chappel, E. Five Figure Mathematical Tables 8vo, 250
Charnock, Mechanical Technology 8vo, 3 50
Charpentier, P. Timber 8vo, *6 oo
Chatley, H. Principles and Designs of Aeroplanes i6mo, o 75
How to Use Water Power i2mo, *i 50
— Gyrostatic Balancing 8vo, *i 25
Child, C. D. Electric Arc 8vo, *2 oo
Christian, M. Disinfection and Disinfectants i2mo, 2 50
Christie, W. W. Beiler-waters, Scale, Corrosion, Foaming 8vo, *3 oo
• Chimney Design and Theory 8vo, *3 oo
Furnace Draft i6mo, o 75
• Water: Its Purification and Use in the Industries 8vo, *2 oo
Church's Laboratory Guide 8vo, 2 50
Clapham, J. H. Woolen and Worsted Industries 8vo, 200
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 7
Clapperton, G. Practical Papermaking 8vo (Reprinting.}
Clark, A. G. Motor Car Engineering.
Vol. I. Construction *4 oo
Vol. II. Design 8vo, *3 50
Clark, C. H. Marine Gas Engines. New Edition 2 oo
Clarke, J. W., and Scott, W. Plumbing Practice.
Vol. I. Lead Working and Plumbers' Materials 8vo, *4 oo
Vol. II. Sanitary Plumbing and Fittings (In Press.")
Vol. III. Practical Lead Working on Roofs (In Press.}
Clarkson, R. P. Elementary Electrical Engineering (In Press.}
Clerk, D., and Idell, F. E. Theory of the Gas Engine .i6mo, o 75
Clevenger, S. R. Treatise on the Method of Government Surveying.
i6mo, morocco, 2 50
Clouth, F. Rubber, Gutta-Percha, and Balata 8vo, *6 oo
Cochran, J. Concrete and Reinforced Concrete Specifications 8vo, *2 50
• Treatise on Cement Specifications 8vo, *i oo
Cocking, W. C. Calculations for Steel-Frame Structures i2mo, *2 50
Coffin, J. H. C. Navigation and Nautical Astronomy i2mo, 3 oo
Colburn, Z., and Thurston, R. H. Steam Boiler Explosions. .. .i6mo, o 75
Cole, R. S. Treatise on Photographic Optics i2mo, 2 oo
Coles-Finch, W. Water, Its Origin and Use .' 8vo, *5 oo
Collins, C. D. Drafting Room Methods, Standards and Forms Svo, 2 oo
Collins^ S. Hoare. Plant Products and Chemical Fertilizers Svo, 3 oo
Collis, A. G. High and Low Tension Switch-Gear Design Svo, *3 50
Switchgear i2mo, o 50
Colver, E. D. S. High Explosives Svo, 12 50
Comstock, D. F., and Troland, L. T. The Nature of Electricity and
Matter Svo, 2 50
Coombs, H. A. Gear Teeth i6mo, o 75
Cooper, W. R. Primary Batteries 8vo, *6 oo
Copperthwaite, W. C. Tunnel Shields 4to, *g oo
Corfield, W. H. Dwelling Houses i6mo, 075
Water and Water-Supply i6mo, o 75
Cornwall, H. B. Manual of Blow-pipe Analysis Svo. *2 50
Cowee, G. A. Practical Safety Methods and Devices Svo, 4 oa
Cowell, W. B. Pure Air, Ozone, and Water i2mo, *a 50
Craig, J. W., and Woodward, W. P. Questions and Answers Abo*t
Electrical Apparatus i2mo, leather, i 50
Craig, T. Motion of a Solid in a Fuel i6mo, o 75
— Wave and Vortex Motion i6mo, o 75
Crehore, A. C. Mystery of Matter and Energy Svo, i oo
— . New Theory of the Atom (In Press.}
Crocker, F. B., and Arendt, M. Electric Motors 8vo, *2 50
Crocker, F. B., and Wheeler, S. S. The Management of Electrical Ma-
chinery I2H10, *I OO
Crosby, E. TJ., Fiske, H. A., and Forster, H. W. Handbook of Fire
Protection i2mo, 4 oo
Cross, C. F., Bevan, E. J., and Sindall, R. W. Wood Pulp and Its
Uses Svo (Reprinting.}
Crosskey, L. R. Elementary Perspective Svo, i 50
8 D. VAN NOSTRAXD CO.'S SHORT TITLE CATALOG
Crosskey, L. R., and Thaw, J. Advanced Perspective 8vo, 2 oo
Culley, J. L. Theory of Arches i6mo, o 75
Gushing, H. C., Jr., and Harrison, N. Central Station Management. ,, *2 oo
Dadourian, H. M. Analytical Mechanics i2mo, *3 oo
— Graphic Statics 8vo, o 75
Danby, A. Natural Rock Asphalts and Bitumens 8vo, *2 50
Darling, E. R. Inorganic Chemical Synonyms ii.mo, i oo
Davenport, C. The Book 8vo, 2 oo
Davey, N. The Gas Turbine 8vq, *4 oo
Davies, F. H. Electric Power and Traction 8vo, *2 oo
— — Foundations and Machinery Fixing i6mo, i oo
Deerr, N. Sugar Cane 8vo, 10 oo
De la Coux, H. The Industrial Uses of Water 8vo, 5 oo
Del Mar, W. A. Electric Power Conductors 8vo, *2 oo
Denny, G. A. Deep-level Mines of the Rand 4to, *io oo
De Roos, J. D. C. Linkages ifcmo, o 75
Derr, W. L. Block Signal Operation Oblong i2mo, *i 50
Desaint, A. Three Hundred Shades and How to Mix Them 8vo, *g oo
De Varona, A. Sewer Qases i6mo, o 75
Devey, R. G. Mill and Factory Wiring i2mo, i oo
Dichmann, Carl. Basic Open Hearth Steel Process i2mo, 4 oo
Dieterich, K. Analysis of Resins, Balsams, and Gum Resins. .. .8vo, *3 50
Dilworth, E. C. Steel Railway Bridges 4to. *4 oo
Dinger, Lieut. H. C. Care and Operation of Naval Machinery. .. lamo, *3 oo
Dixon, D. B. Machinist's and Steam Engineer's Practical Calculator.
i6mo, morocco, i 25
Dommett, W. E. Motor Car Mechanism 12010, *2 oo
Dorr, B. F. The Surveyor's Guide and Pocket Table-book.
i6mo, morocco, 2 oo
Draper, C. H. Heat and the Principles of Thermo-Dynamics. . i2mo, 2 25
Draper, E. G. Navigating the Ship 12010, 2 oo
Dubbel, H. High Power Gas Engines 8vo, *5 oo
Dumesny, P., and Noyer, J. Wood Products, Distillates, and Extracts.
8vo, *5 oo
Duncan, W. G., and Penman, D. The Electrical Equipment of Collieries.
8vo, *5 oo
Dunkley, W. G. Design of Machine Elements. Two volumes. .8 vo,each, 2 oo
Dunstan, A. E., and Thole, F. B. T. Textbook of Practical Chemistry.
i2mo, *i 40
Durham, H. W. Saws. 8vo, 2 50
Duthie, A. L. Decorative Glass Processes 8vo, 2 50
Dwight, H. B. Transmission Line Formulas 8vo, *2 oo
Dyke, A. L. Dyke's Automobile and Gasoline Engine Encyclopedia,
8vo, 5 oo
Dyson, S. S. A Manual of Chemical Plant. 12 parts. .. -4to, paper, 7 50
Dyson, S. S., and Clarkson, S. S. Chemical Woiks 8vo, *g oo
Eccles, W. H. Wireless Telegraphy and Telephony i2mo, *8 80
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 9
Eck, J. Light, Radiation and Illumination 8vo, 250
Eddy, L. C. Laboratory Manual of Alternating Currents i2mo, o 50
Edelman, P. Inventions and Patents i2mo, *i 50
Edgctmbe, K. Industrial Electrical Measuring Instruments 8vo, 5 oo
Edler, R. Switches and Switchgear 8vo, 4 oo
Eissler, M. The Metallurgy of Gold 8vo, 9 oo
The Metallurgy of Silver 8vo, 4 oo
The Metallurgy of Argentiferous Lead 8vo, 6 25
A Handbook on Modern Explosives 8vo, 5 oo
Ekin, T. C. Water Pipe and Sewage Discharge Diagrams folio, *3 oo
Electric Light Carbons, Manufacture of 8vo, i oo
Eliot, C. W., and Storer, F. H. Compendious Manual of Qualitative
Chemical Analysis i2mo, *i 25
Ellis, C. Hydrogenation of Oils 8vo, 7 50
Ultraviolet Light, Its Applications in Chemical Arts i2mo,
(In Press}
and Meigs, J. V. Gasolene and Other Motor Fuels.. (In Press.}
Ellis, G. Modern Technical Drawing 8vo, *2 oo
Ennis, Wm. D. Linseed Oil and Other Seed Oils 8vo, 5 oo
Applied Thermodynamics 8vo, 5 oo
Flying Machines To-day i2mo, *i 50
Vapors for Heat Engines i2mo, *i oo
Ermen, W. F. A. Materials Used in Sizing 8vo, *2 oo
'Erwin, M. The Universe and the Atom i2mo (Reprinting.}
Ewing, A. J. Magnetic Induction in Iron 8vo, 5 oo
Fairchild, J. F. Graphical Compass Conversion Chart and Tables... o 50
Fairie, J. Notes on Lead Ores i2mo, *o 50
— Notes on Pottery Clays i2mo, *2 oo
Fairley, W., and Andre, Geo. J. Ventilation of Coal Mines. .. .i6mo, o 75
Fairweather, W. C. Foreign and Colonial Patent Laws 8vo, *3 oo
Falk, K. G. Chemical Reactions: Their Theory and Mechanism.
(In Press.}
Fanning, J. T. Hydraulic and Water-supply Engineering 8vo, *5 oc
Farnsworth, P. V. Shop Mathematics i2mo (In Press.}
Fay, I. W. The Coal-tar Dyes 8vo, 5 oa
Fernbach, R. L. Glue and Gelatine > 8vo, *3 oo
Findlay, A. The Treasures of Coal Tar i2mo, 2 oo
Firth, J. B. Practical Physical Chemistry i2mo] i 25
Fischer, E. The Preparation of Organic Compounds i2mo, i 50
Fisher, H. K. C., and Darby, W. C. Submarine Cable Testing. . .8vo, 4 oo
^leischmann, W. The Book of the Dairy 8vo, 4 50
Fleming, J. A. The Alternate-current Transformer. Two Volumes. 8vo.
Vol. I. The Induction of Electric Currents *6 50
Vol, II. The Utilization of Induced Currents 6 50
Propagation of Electric Currents 8vo, 3 50
A Handbook for the Electrical Laboratory and Testing Room. Two
Volumes 8vo, each, *6 5°
Fleury, P. Preparation and Uses of White Zinc Paints 8vo, 3 oo
Flynn, P. J. Flow of Water : 12mo> 0 75
Hydraulic Tables i6tno, o 75
10 D. V*.N NOSTRAND CO.'S SHORT TITLE CATALOG
Foster, H. A. Electrical Engineers' Pocket-book. (Seventh Edition.)
i2mo, leather, 5 oo
— Engineering Valuation of Public Utilities and Factories 8vo, *3 oo
Fowle, F. F. Overhead Transmission Line Crossings 12 mo, *i 50
The Solution of Alternating Current Problems .... .8vo (In Press.)
Fox, W. G. Transition Curves i6mo, o 75
Fox, W., and Thomas, C. W. Practical Course in Mechanical Draw-
ing 1 2010, i 25
Foye, J. C. Chemical Problems i6mo, o 75
— Handbook of Mineralogy i6mo, 075
Francis, J. B. Lowell Hydraulic Experiments 4to, 15 oo
Franzen, H. Exercises in Gas Analysis i2mo, *i oo
Fraser, E. S., and Jones, R. B. Motor Vehicles and Their Motors,
Svo, fabrikoid, 2 oo
Freudemacher, P. W. Electric Mining Installations iamo, i oo
Friend, J. N. The Chemistry of Linseed Oil i2mo, i oo
Fritsch, J. Manufacture of Chemical Manures .8vo, 5 oo
Frye, A. I. Civil Engineers' Pocket-book i2mo, leather, *5 oo
Fuller, G. W. Investigations into the Purification of the Ohio River.
4to, *io oo
Furaell, J. Paints, Colors, Oils, and Varnishes Svo.
Gant, L. W. Elements of Electric Traction Svo, *2 50
Garcia, A. J. R. V. Spanish-English Railway Terms Svo, 3 co
Gardner, H. A. Paint Researches, and Their Practical Applications,
Svo, *s oo-
Garforth, W. E. Rules for Recovering Coal Mines after Explosions and
Fires i2mo, leather, i 50
Garrard, C. C. Electric Switch and Controlling Gear Svo, *6 oo
Gaudard, J. Foundations i6mo, o 75
Gear, H. B., and Williams, P. F. Electric Central Station Distribution
Systems Svo, *s 50
Geerligs, H. C./ P. Cane Sugar and Its Manufacture Svo, *6 oo
Chemical Control in Cane Sugar Factories 4to, 5 oo
Geikie, J. Structural and Field Geology Svo, 4 50
— Mountains. Their Growth, Origin and Decay Svo, 4 50
— The Antiquity of Man in Europe Svo, *s oo
Georgi, F., and Schubert, A. Sheet Metal Working Svo, 3 50
Gerhard, W. P. Sanitation, Watersupply and Sewage Disposal of Country
Houses i2mo, *2 oo
Gas Lighting i6mo, o 75
— Household Wastes i6mo, o 75
— House Drainage i6mo, o 75
— Sanitary Drainage of Buildings i6mo, o 75
Gerhardi, C. W. H. Electricity Meters Svo, *y 20
Geschwind, L. Manufacture of Alum and Sulphates Svo, 5 oo
Gibbings, A. H. Oil Fuel Equipment for Locomotives. Svo.
(Reprinting.}
Gibbs, W. E. Lighting by Acetylene . . 12010, *i 50
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG n
Gibson, A. H. Hydraulics and Its Application 8vo, 6 oo
• Water Hammer in Hydraulic Pipe Lines i2mo, 2 50
Gibson, A. H., and Ritchie, E. G. Circular Arc Bow Girder 4to, *s 50
Gilbreth, F. B. Motion Study i2mo, *2 oo
— Primer of Scientific Management i2mo, *i oo
Gillmore, Gen. Q. A. Roads, Streets, and Pavements iamo, i 25
Godfrey, E. Tables for Structural Engineers i6mo, leather, *2 50
Golding, H. A. The Theta-Phi Diagram i2mo, *2 oo
Goldschmidt, R. Alternating Current Commutator Motor 8vo, *3 oo
Goodchild, W. Precious Stones 8vo, 2 50
Goodell, J. M. The Location, Construction and Maintenance of
Roads 8vo, 2 oo
Goodeve, T. M. Textbook on the Steam-engine i2mo, 2 50
Gore, G. Electrolytic Separation of Metals 8vo, 4 50
Gould, E. S. Arithmetic of the Steam-engine i2mo, i oo
— Calculus i6mo, o 75
— High Masonry Dams i6mo, o 75
Gould, E. S. Practical Hydrostatics and Hydrostatic Formulas. .16 mo, o 75
Gratacap, L. P. A Popular Guide to Minerals 8vo, *2 oo
Gray, H. H. Gas-Works Products 8vo (/;/ Prrss.)
Gray, J. Electrical Influence Machines i2mo, 2 oo
Marine Boiler Design i2mo (Reprinting.)
Greenhill, G. Dynamics of Mechanical Flight 8vo, *2 50
Greenwood, H. C. The Industrial Gases 8vo (/// Press.}
Gregorius, R. Mineral Waxes i2mo, 3 oo
Grierson, R. Some Modern Methods of Ventilation 8vo, *s oo
Griffiths, A. B. A Treatise on Manures i2mo (Reprinting.}
Gross, E. Hops 8vo, *5 oo
Grossman, J. Ammonia and Its Compounds i2mo, i 50
Groth, L. A. Welding and Cutting Metals by Gases or Electricity.
8vo, 2 50
Grover, F. Modern Gas and Oil Engines .8vo, *3 oo
Grunerf A. Power-loom Weaving 8vo, *s 50
Grunsky, C. E. Topographic Stadia Surveying i6mo, 2 oo
Guldner, H. Internal Combustion Engines (In Press.)
Gunther, C. 0. Integration 8vo, i 50
Gurden, R. L. Traverse Tables folio, half morocco, *y 50
Guy, A. E. Experiments on the Flexure of Beams 8vo, *i 25.
Haenig, A. Emery and Emery Industry 8vo, *2 50
Hainbach, R. Pottery Decoration i2mo, 3 50
Hale, A. J. The Manufacture of Chemicals by Electrolysis. 8vo,
(In Press.)
Hale, W. J. Calculations of General Chemistry i2mo, i 50
Hall, C. H. Chemistry of Paints and Paint Vehicles i2mo, *2 oo
Hall, R. H. Governors and Governing Mechanism i2mo, *2 50
Hall, W. S. Elements of the Differential and Integral Calculus 8vo, 2 75
— Descriptive Geometry 8vo volume and a 4to atlas, 4 oo
Haller, G. F., and Cunningham, E. T. The Tesla Coil i2mo, *i 25
Halsey, F. A. Slide Valve Gears i2mo, i 50
— The Use of the Slide Rules i6mo, 075
Worm and Spiral Gearing i6mo, o 75
12 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Hancock, H. Textbook of Mechanics and Hydrostatics 8vo, i 50
Hardy, E. Elementary Principles of Graphic Statics i2mo, *i 50
flaring, H. Engineering Law.
Vol. I. Law of Contract 8vo, *4 oo
Harper, J. H. Hydraulic Tables on the Flow of Water i6mo, *2 oo
Harris, S. M. Practical Topographical Surveying (In Press.)
Harrow, B. Eminent Chemists of Our Times: Their Lives and Work.
(In Press.)
Haskins, C. H. The Galvanometer and Its Uses i6mo, i 50
Hatt, J. A. H. The Colorist square i2mo, *i 50
Hausbrand, E. Drying by Means of Air and Steam 12010, 2 50
— Evaporating, Condensing and Cooling Apparatus 8vo, 6 oo
Hausmann, E. Telegraph Engineering 8vo, *3 oo
Hausner, A. Manufacture of Preserved Foods and Sweetmeats. .. .8vo, 3 50
Hawkesworth, J. Graphical Handbook for Reinforced Concrete Design.
4to, 2 oo
Hay, A. Continuous Current Engineering 8vo, ;: 2 50
Hayes, H. V. Public Utilities, Their Cost New and Depreciation. . .8vo, *2 oo
— Public Utilities, Their Fair Present Value and Return 8vo, *2 oo
Heath, F. H. Chemistry of Photography 8vo.. (In Press.)
Heather, H. J. S. Electrical Engineering 8vo, 4 50
Heaviside, 0. Electromagnetic Theory. Vols. I and II....8vo, each,
(Reprinting.)
Vol. Ill 8vo (Reprinting.)-
Heck, R. C. H. The Steam Engine and the Turbine 8vo, 4 50
Steam-Engine and Other Steam Motors. Two Volumes.
Vol. I. Thermodynamics and the Mechanics 8vo, 4 50
Vol. II. Form, Construction, and Working 8vo, 550
Notes on Elementary Kinematics 8vo, boards, *i oo
Graphics of Machine Forces 8vo, boards, *i oo
Heermann, P. Dyers' Materials i2mo, 3 oo
Hellot, Macquer and D'Apligny. Art of Dyeing Wool, Silk and Cotton. 8vo, *2 oo
Bering, C., and Getman, F. H. Standard Tables of Electro-Chemical
Equivalents i2mo, *2 oo
Bering, D. W. Essentials of Physics for College Students 8vo, 2 25
Herington, C. F. Powdered Coal as Fuel 8vo, 3 oo
Herrmann, G. The Graphical Statics of Mechanism i2mo, 2 oo
Herzfeld, J. Testing of Yarns and Textile Fabrics 8vo.
(New Edition in Preparation.)
Hildenbrand, B. W. Cable-Making i6mo, o 75
Hilditch, T. P. A Concise History of Chemistry i2mo, *i 50
Hill, M. J. M. The Theory of Proportion 8vo, *2 50
Hillhouse, P. A. Ship Stability and, Trim .8vo, 4 50
Hiroi, I. Plate Girder Construction i6mo, o 75
— ^Statically-Indeterminate Stresses i2mo, 2 50
Hirshf eld, C. F. Engineering Thermodynamics i6mo, o 75
Hoar, A. The Submarine Torpedo Boat i2mo, *2 oo
Hobart, H. M. Heavy Electrical Engineering 8vo, *4 50
— Design of Static Transformers i2mo, 250
— Electricity 8vo, *2 oo
— Electric Trains 8vo, *2 50
Electric Propulsion of Ships 8vo, *2 50
D. VAN NQSTRAND CO.'S SHORT TITLE CATALOG 13
Hobart, J. F. Hard Soldering, Soft Soldering and Brazing I2mo, i 25
Hobbs, W. R. P. The Arithmetic of Electrical Measurements. .. .i2mo, o 75
Hoff, J. N. Paint and Varnish Facts and Formulas i2mo, i 50
Hole, W. The Distribution of Gas 8vo, *8 50
Hopkins, N. M. Model Engines and Small Boats i2mo, i 25
— The Outlook for Research and Invention i2mo. 2 oo
Hopkinson, J., Shoolbred, J. N., and Day, R. E. Dynamic Electricity.
i6mo. o ?!>
Homer, J. Practical Ironf ounding 8vo, *2 oo
— Gear Cutting, in Theory and Practice 8vo (Reprinting.)
Houghton, C. E. The Elements of Mechanics of Materials i2mo, 2 50
Houstoun, R. A. Studies in Light Production 12010, 2 oo
Hovenden, F. Practical Mathematics for Young Engineers 12010, *i 50
Howe, G. Mathematics for the Practical Man i2mo, i 50
Koworth, J. Repairing and Riveting Glass, China and Earthenware.
8vo, paper, *o 50
Hoyt, W. E. Chemistry by Experimentation 8vo, *» 70
Hubbard, E. The Utilization of Wood-waste 8vo, *2 50
Hiibner, J. Bleaching and Dyeing of Vegetable and Fibrous Materials.
8vo (Reprinting.).
Hudson, 0. Ff Iron and Steel 8vo, •<. ^
Humphreys, A. C. The Business Features of Engineering Practice . 8vo, 2 50-
Hunter, A. Bridge Work 8vo. (In Press.)
Hurst, G. H. Handbook of the Theory of Color 8vot *3 50
Dictionary of Chemicals and Raw Products 8vo, *5 oo
Lubricating Oils, Fats and Greases 8vo, *$ oo
Soaps , 8vo, *6 oo
Hurst, G. H., and Simmons, W. H. Textile Soaps and Oils 8vo, 3 50
Hurst, H. E.t and Lattey, R. T. Text-book of Physics 8vo, *3 oo
Also published in three parts.
Part I. Dynamics and Heat i 50
Part II. Sound and Light , 150
Part in. Magnetism and Electricity *i 50
Hutchinson, R. W., Jr. Long Distance Electric Power Transmission.
i2mo, *3 oo
Hutchinson, R. W., Jr., and Thomas, W. A. Electricity in Mining. i2mo.
(In Press.)
Hyde, E. W. Skew Arches i6mo. o 75
Hyde, F. S. Solvents, Oils, Gums, Waxes 8vo, *2 oo
Induction Coils i6mo. o 75
Ingharn, A. E. Gearing. A practical treatise 8vo, *2 50
Ingle, H. Manual of Agricultural Chemistry 8vo (In Press.}
Inness, C. H. Problems in Machine Design i2mo, *3 oo
— Centrifugal Pumps i2mo, *3 oo
The Fan ...,,, i2mo, *4 oo
Jacob, A., and Gould, E. S. On the Designing and Construction of
Storage Reservoirs i6mo. o 75
Jacobs, F. B. Cam Design and Manufacture ( In Press.)
I4 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
James, F. D. Controllers for Electric Motors 8vo. * oo
Jehl, F. Manufacture of Carbons 8vo. 5 oo
Jennings, A. S. Commercial Paints and Painting 8vo. 2 so
Jennison, F. H. The Manufacture of Lake Pigments. .8vo (In Press.)
Jepson, G. Cams and the Principles of their Construction 8vo, *i 50
Mechanical Drawing 8vo (In Preparation.)
Jervis-Smith, F. J. Dynamometers 8vo. 4 oo
Jockin, W. Arithmetic of the Gold and Silversmith 12010, *i oo
Johnson, C. H., and Earle, R. P. Practical Tests for the Electrical
Laboratory ( /;/ Press.)
Johnson, J. H. Arc Lamps and Accessory Apparatus i2mo, o 75
Johnson, T. M. Ship Wiring and Fitting i2mo (Reprinting.)'
Johnston, J. F. W., and Cameron, C. Elements of Agricultural Chemistry
and Geology iimo, 2 60
Joly, J. Radioactivity and Geology i2mo (Reprinting.)
Jones, H. C. Electrical Nature of Matter and Radioactivity i2mo, *2 oo
Nature of Solution 8vo, *3 50
New Era in Chemistry i2mo, *2 oo
Jones, J. H. Tinplate Industry 8vo, *s oo
Jones, M. W. Testing Raw Materials Used in Paint i2mo, *2 50
Jordan, L. C. Practical Railway Spiral i2mo, leather, *i 50
Juptner, H. F. V. Siderclogy: The Science of Iron 8vo, *s oo
Kapp, G. Alternate Current Machinery i6mo, o 75
Kapper, F. Overhead Transmission Lines. 4to, ^400
Keim, A. W. Prevention of Dampness in Buildings 8vo, *2 50
Keller, S. S., and Knox, W. E. Analytical Geometry and Calculus. .. 2 oo
Kemble, W. T., and Underbill, C. R. The Periodic Law and the Hydrogen
Spectrum 8vo, paper, *o 50
Kemp, J. F. Handbook of Rocks 8vo, *i 50
Kennedy, A. B. W., and Thurston, R. H. Kinematics of Machinery.
i6mo, o 75
Kennedy, A. B. W., Unwin, W. C., and Idell, F. E. Compressed Air.
i6mo, o 75
Kennedy, R. Flying Machines ; Practice and Design i2mo, 2 50
— Principles of Aeroplane Construction 8vo, *2 oo
Kent. W. Strength of Materials i6mo, o 75
Kershaw, J. B. C. Fuel, Water and Gas Analysis. .8vo (In Press.)
Electrometallurgy 8vo, 2 50
Electro-Thermal Methods of Iron and Steel Production 8vo, *3 oo
Kinzbrunner, C. Continuous Current Armatures 8vo, i 50
- Testing of Alternating Current Machines 8vo, *2 oo
Kinzer, H., and Walter, K. Theory and Practice of Damask Weaving,
8vo, 4 oo
Kirkaldy, A.. W., and Evans, A. D. History and Economics of
Transport 8vo, *s oo
Kirkbride, J. Engraving for Illustration 8vo, *i oo
Kirschke, A. Gas and Oil Engines i2mo, *i 50
D VAN NOSTRAND CO.'S SHORT TITLE CATALOG 15
Klein, J. F. Design of a High-speed Steam-engine 8vo, *5 oo
Physical Significance of Entropy 8vo, *i 50
Klingenberg, G. Large Electric Power Stations 4to, *5 oo
Knight, R.-Adm. A. M. Modern Seamanship 8vo, *6 50
Pocket Edition i2mo, f abrikoid, 3 oo
Knott, C. G., and Mackay, J. S. Practical Mathematics 8vo, 2 50
Knox, J. Physico-Chemical Calculations. i2mo, i 50
Fixation of Atmospheric Nitrogen. . .7 i2mo, i oo
Koester, F. Steam-Electric Power Plants 4to, *5 oo
Hydroelectric Developments and Engineering 4to, *5 oo
Koller, T. The Utilization of Waste Products 8vo, *5 oo
— Cosmetics 8vo, *2 50
Koppe, S. W. Glycerine xarno, *s 50
Kozmin, P. A. Flour Milling 8vo, 750
Krauch, C. Chemical Reagents 8vo, ^ oo
Kremann, R. Application of the Physico-Chemical Theory to Tech-
nical Process and Manufacturing Methods 8vo, 3 oo
Kretchmar, K. Yarn and Warp Sizing 8vo, *$ oo
Laff argue, A. Attack in Trench Warfare i6mo, o 50
Lallier, E. V. Elementary Manual of the Steam Engine i2mo, *2 oo
Lambert, T. Lead and Its Compounds 8vo, *3 50
— Bone Products and Manures 8vo, *3 50
Lamborn, L. L. Cottonseed Products 8vo, 4 oo
Modern Soaps, Candles, and Glycerin 8vo, **j 50
Lamprecht, R. Recovery Work After Pit Fires .8vo, 5 oo
Lanchester, F. W. Aerial Flight. Two Volumes. 8vo.
Vol. I. Aerodynamics *6 oo
Vol. II. Aerodonetics *6 oo
Lanchester, F. W. The Flying Machine 8vo, *3 oo
Industrial Engineering: Present and Post- War Outlook. . . i2mo, i oo
Lange, K. R, By-Products of Coal-Gas Manufacture xamo, 2 50
La Rue, B. F. Swing Bridges i6mo, o 75
Lassar-Cohn, Dr. Modern Scientific Chemistry i2mo, 2 25
Latimer, L. H., Field, C. J., ,and Howell, J. W. Incandescent Electric
Lighting i6mo, o 75
Latta, M. N. Handbook of American Gas-Engineering Practice. .8vo, 5 oo
American Producer Gas Practice 4to, *6 oo
Laws, B. C. Stability and Equilibrium of Floating Bodies 8vo, 4 50
Law&on, W. R. British Railways. A Financial and Commercial
Survey 8vo, 200
Leask, A. R. Refrigerating Machinery i2mo (Reprinting.)
Lecky, S. T. S. "Wrinkles" in Practical Navigation 8vo, 10 oo
— Pocket Edition i2mo, 5 oo
— Danger Angle i6mo, 2 50
Le Doux, M. Ice-Making Machines i6mo, o 7$
Leeds, C. C. Mechanical Drawing for Trade Schools oblong 4to, 2 25
Mechanical Drawing for High and Vocational Schools 4to, i 50
Principles of Engineering Drawing 8vo (In 'Press.)
Lefevre, L, Architectural Pottery 4to, 7 oc
Lehner, S, Ink Manufacture 8vo, 2 50
Lemstrom, S. Electricity in Agriculture and Horticulture 8vo, *i 50
Letts, E. A. Fundamental Problems in Chemistry 8vo, *2 oo
Le Van, W. B. Steam-Engine Indicator i6mo, o 7$
!6 D. VAX XOSTRAXD CO.'S SHORT ^ITLE CATALOG
Lewes, V. B. Liquid and Gaseous Fuels Svo, 3 oo
— Carbonization of Coal 8vo, : 5 oo
Lewis Automatic Machine Rifle ; Operation of i6mo, *o Go
Licks, H. E. Recreations in Mathematics i2mo, i 50
Lieber, B. F. Lieber's Five Letter American Telegraphic Code .8vo, ^15 oo
. Spanish Edition 3vo, ^15 oo
— French Edition 8vo, "15 oo
— Terminal Index 8vo, *2 50
— Lieber's Appendix folio, *i5 oo
— Handy Tables 4to, *2 50
Bankers and Stockbrokers' Code and Merchants and Shippers'
Blank Tables 8vo, *i$ oo
— 100,000,000 Combination Code .8vo, *io oo
Livermore, V. P., and Williams, J. How to Become a Competent Motor-
man i2mo, *i oo
Livingstone, R. Design and Construction of Commutators 8vo, 450
— Mechanical Design and Construction of Generators 8vo, 4 50
Lloyd, S. L. Fertilizer Materials i-zmo, 2 oo
Lockwood, T. D. Electricity; Magnetism, and Electro-telegraph. .... STO, 2 50
— Electrical Measurement and the Galvanometer i2mo, o 75
Lodge, O. J. Elementary Mechanics i2mo, i 50
Loewenstein, L. C., and Crissey, C. P. Centrifugal Pumps.. 5 oo
Lomax, J. W. Cotton Spinning 12010, i 50
Lord, R. T. Decorative and Fancy Fabrics Svo, *3 50
Loring, A. E. A Handbook of the Electromagnetic Telegraph. . . i6mo, o 75
Lowy, A. Organic Type Formulas o 10
Lubschez, B. J- Perspective 12010, *i 50
Lucke, C. E. Gas Engine Design Svo, *?. oo
- — Power Plants: Design, Efficiency, and Power Costs. 2 vols.
(In Preparation.)
Luckiesh, M. Color and Its Application Svo, 3 50
— Light and Shade and Their Applications 8vo, 3 oo
— Visual Illusions (In Preparation. )
Lunge, G. Coal-tar and Ammonia. Three Volumes .8vo, *25 oo
— Technical Gas Analysis Svo, *4 $&
Manufacture of Sulphuric Acid and Alkali. Four Volumes 8vo,
Vol. I. Sulphuric Acid. In three parts (Reprinting.)
Vol. I. Supplement Svo (Reprinting.)
Vol. II. Salt Cake, Hydrochloric Acid and Leblanc Soda. In two
parts (In Press. )
Vol. III. Ammonia Soda (In Press.)
Vol. IV. Electrolytic Methods (In Press.)
— Technical Chemists' Handbook tamo, leather, *4 oo
— Technical Methods of Chemical Analysis.
Vol. I. In two parts Svo, *i$ oo
Vol. II. In two parts , 8vo, *i8 oo
Vol. III. In two parts Svo, *i8 oo
The set (3 vols.) complete *5o oo
Luquer, L. M. Minerals in Rock Sections .. . .8vo, *i 5»
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 17
MacBride, J. D. A Handbook of Practical Shipbuilding,
i2mo, fabrikoid, 2 oo
Macewen, H. A. Food Inspection 8vo, *2 50
Mackenzie, N. F. Notes on Irrigation Works 8vo, *2 50
Mackie, J. How to Make a Woolen Mill Pay 8vo, *2 oo
Maguire, Wm. R. Domestic Sanitary Drainage and Plumbing .... 8vo, 4 oo
Malcolm, H. W. Submarine Telegraph Cable 9 oo
Malinovzsky, A. Analysis of Ceramic Materials and Methods of
Calculation (In Press.}
Mallet, A. Compound Engines i6mo,
Mansfield, A. N. Electro-magnets i6mo, o 75
Marks, E. C. R. Construction of Cranes and Lifting Machinery. i2mo, *2 75
Manufacture of Iron and Steel Tubes i2mo, 2 50
— Mechanic*! Engineering Materials 12010, *i 50
Marks, G. C. Hydraulic Power Engineering 8vo, 4 50
Marlow, T. G. Drying Machinery and Practice. .. .8vo (Reprinting.)
Marsh, C. F. Concise Treatise on Reinforced Concrete 8vo, *2 50
Reinforced Concrete Compression Member Diagram. Mounted on
Cloth Boards *i .50
Marsh, C. F., and Dunn, W. Manual of Reinforced Concrete and Con-
crete Block Construction i6mo, cloth, 2 oo
Marshall, W. J., and Sankey, H. R. Gas Engines 8vo, 2 oo
Martin, G. Triumphs and Wonders of Modern Chemistry 8vo, *3 oo
— Modern Chemistry and Its Wonders 8vo, *s oo
Martin, N. Properties and Design of Reinforced Concrete 8vo, i 50
Martin, W. D, Hints to Engineers i2mo, 2 oo
Massie, W. W., and Underbill, C. R. Wireless Telegraphy and Telephony.
i2mo, *i oo
Mathot, R. E. Internal Combustion Engines 8vo, 5 oo
Maurice, W. Electric Blasting Apparatus and Explosives 8vo, *3 50
Shot Firer*s Guide 8vo, *i 50
Maxwell, F. Sulphitation in White Sugar Manufacture i2mo, 4 oo
Maxwell, J. C. Matter and Motion i6mo, o 75
Maxwell, W. H., and Brown, J. T. Encyclopedia of Muni.ipal and Sani-
tary Engineering 4to, *io oo
Mayer, A. M. Lecture Notes on Physics 8vo, 2 oo
McCracken, E. M., and Sampson, C. H. Course in Pattern Making.
(In Press.)
McCullough, E. Practical Surveying i2mo, 2 50
McCullough, R. S. Mechanical Theory of Heat 8vo, 3 50
McGibbon, W. C. Indicator Diagrams for Marine Engineers 8vo, "3 50
— Marine Engineers' Drawing Book oblong 4to, *2 50
McGibbon, W. C. Marine Engineers Pocketbook i2mo, *4 50
Mclntosh, J. G. Technology of Sugar 8vo, *6 oo
— Industrial Alcohol ; 8vo, *3 50
Manufacture of Varnishes and Kindred Industries. Three Volumes.
8vo.
Vol. I. Oil Crushing, Refining and Boiling 7 oo
Vol. II. Varnish Materials and Oil Varnish Making. (Reprinting.)
Vol. III. Spirit Varnishes and Materials (Reprinting.)
McKay, C. W. Fundamental Principles of the Telephone Business.
8vo. (In Press.)
i8 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
McKillop, M., and McKillop, A. D. Efficiency Methods i2mo, i 50
UcKnight, J. D., and Brown, A. W. Marine Multitubular Boilers.... *2 50
McMaster, J. B. Bridge and Tunnel Centres i6mo, o 75
McMechen, F. L. Tests for Ores, Minerals and Metals i2mo, *i co
McNair, Jas. B. Citrus By-Products : (hi press.)
Meade, A. Modern Gas Works Practice 8vo, *8 50
Melick, C. W. Dairy Laboratory Guide 12010, *i 25
"Mentor." Self-Instruction for Students in Gas Supply. i2mo.
Elementary 2 50
Advanced 2 50
- — Self-Instruction for Students in Gas Engineering. i2mo.
Elementary 2 oo
Advanced 2 oo
Merivale, J. H. Notes and Formulae for Mining Students i2mo, i oo
Merritt, Wm. H. Field Testing for Gold and Silver i6mo, leather, 2 oo
Mertens. Tactics and Technique of River Crossings 8vo, 2 50
Mierzinski, S. Waterproofing of Fabrics 8vo, 2 50
Miessner, B. F. Radio Dynamics i2mo, *2 oo
Miller, G. A. Determinants . . i6mo,
Miller, W. J. Introduction to Historical Geology i2mo, 2 25
Milrpy, M. E. W. Home Lace-making i2mo, *i oo
Mills, C. N. Elementary Mechanics for Engineers 8vo, *i oo
Mitchell, C. A. Mineral and Aerated Waters 8vo, *3 oo
Mitchell, C. A., and Prideaux, R. M. Fibres Used in Textile and Allied
Industries .'../ ...8vo, 3 50
Mitchell, C. F., and G. A. Building Construction and Drawing. i2mo.
Elementary Course 2 oo
Advanced Course 3 oo
Monckton, C. C. F. Radiotelegraphy 8vo, 200
Monteverde, R. D. Vest Pocket Glossary of English-Spanish, Spanish-
English Technical Terms 64mo, leather, *i oo
Montgomery, J. H. Electric Wiring Specifications i6mo, *i oo
Moore, E. C. S. New Tables for the Complete Solution of Ganguillet and
Kutter's Formula 8vo, *6 oo
Moore, Harold. Liquid Fuel for Internal Combustion Engines. . .8vo, 5 oo
Morecroft, J. H., and Hehre, F. W. Short Course in Electrical Testing.
8vo, i 75
Morgan, A. P. Wireless Telegraph Apparatus for Amateurs I2mo, *i 50
Morrell, R. S., and Waele, A. E. Rubber, Resins, Paints and Var-
nishes 8vo (In Press.)
Moses, A. J. The Characters of Crystals 8vo, *2 oo
— and Parsons, C. L. Elements of Mineralogy 8vo, *3 50
Moss, S. A. Elements of Gas Engine Design i6mo, o 75
— -The Lay-out of Corliss Valve Gears i6mo, o 75
Mulford, A. C. Boundaries and Landmarks i2mo, *i oo
Mulford, A. C. Boundaries and Landmarks 12010, i oo
Munby, A. E. Chemistry and Physics of Building Materials. .. .8vo, 2 50
Murphy, J. G. Practical Mining i6mo, i oo
Murray, B. M. Chemical Reagents 8vo ( In Press.)
Murray, J. A. Soils and Manures 8vo, 200
Nasmith, J. The Student's Cotton Spinning 8vo, 4 50
Recent Cotton Mill Construction i2mo, 3 oo
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 19
tieave, G. B., and Heilbron, I. M. Identification of Organic Compounds.
i2mo, i 50
Neilson, R. M. Aeroplane Patents 8vo, *2 oo
Kerz, F. Searchlights 8vo (Reprinting.)
Newbigin, M. I., and Flett, J. S. James Geikie, the Man and the
Geologist 8vo, 3 50
Newbiging, T. Handbook for Gas Engineers and Managers 8vo, 7 50
Newell, F. H., and Drayer, C. E. Engineering as a Career. .i2mo, cloth, *i oo
Nicol, G. Ship Construction and Calculations 8vo, *io oo
Nipher, F. E. Theory of Magnetic Measurements i2mo, i oo
Nisbet, H. Grammar of Textile Design 8vo, 7 50
Nolan, H. The Telescope i6mo, o 75
Norie, J. W. Epitome of Navigation (2 Vols.) octavo, 15 oo
— A Complete Set of Nautical Tables with Explanations of Their
Use octavo, 6 50
North, H. B. Laboratory Experiments in General Chemistry 12010, *i oo
<^
O'Connor, H. The Gas Engineer's Pocketbook i2mo, leather, 400
Ohm, G. S., and Lockwood, T. D. Galvanic Circuit i6mo, o 75
Olsen, J. C. Text-book of Quantitative Chemical Analysis 8vo, 400
Ormsby, M. T. M. Surveying i2mo, 2 oo
Oudin, M. A. Standard Polyphase Apparatus and Systems 8vo, *3 oo
Pakes, W. C. C., and Nankivell, A. T. The Science of Hygiene . .8vo, *i 75
Palaz, A. Industrial Photometry -. 8vo, 4 oo
Palmer, A. R. Electrical Experiments i2mo, o 75
— Magnetic Measurements and Experiments i2mo, o 75
Pamely, C. Colliery Manager's Handbook 8vo, *io oo
Parker, P. A. M. The Control of Water 8vo, 600
Parr, G. D. A. Electrical Engineering Measuring Instruments. .. .8vo, *3 50
Parry, E. J, Chemistry of Essential Oils and Artificial Perfumes.
Vol. I. Monographs on Essential Oils 9 oo
Vol. II. Constituents of Essential Oils, Analysis 7 oo
Foods and Drugs. Two Volumes.
Vol. I. The Analysis of Food and Drugs 8vo, 950
Vol. II. The Sale of Food and Drugs Acts 8vo, 3 50
— and Coste, J. H. Chemistry of Pigments .8vo, *5 oo
Parry, L. Notes on Alloys 8vo, *s 50
— Metalliferous Wastes 8vo, *2 50
— Analysis of Ashes and Alloys 8vo, *2 50
Parry, L. A. Risk and Dangers of Various Occupations 8vo, *3 50
Parshall, H. F., and Hobart, H. M. Electric Railway Engineering . 4to, 7 50
Parsons, J. L. Land Drainage 8vo, *i 50
Parsons, S. J. Malleable Cast Iron 8vo (Reprinting.)
Partington, J. R. Higher Mathematics for Chemical Students. .i2mo, 2 50
Textbook of Thermodynamics 8vo, *4 oo
— The Alkali Industry 8vo, 3 oo
Patchell, W. H. Electric Power in Mines 8vo, *4 oo
Paterson, G. W. L. Wiring Calculations i2mo, *2 50
— Electric Mine Signalling Installations i2mo, *i 50
Patterson, D. The Color Printing of Carpet Yarns 8vo, *3 50
Color Matching on Textiles 8vo, *3 50
Textile Color Mixing 8vo, *3 50
20 D. VAN NOSTRANt) CO.'S SHORT TITLE CATALOG
Paulding, C. P. Condensation of Steam in Covered and Bare Pipes. 8vo, *2 oo
- Transmission of Heat through Cold-storage Insulation i2mo, *i oo
Payne, D. W. Iron Founders' Manual 8vo, 4 oo
Peddle, R. A. Engineering and Metallurgical Books 12010, *i 50
Peirce, B. System of Analytic Mechanics 4to, 10 oo
— Linear Associative Algebra 4to, 2 50
Perkin, F. M., and Jaggers, E. M. Elementary Chemistry. ...i2mo, i co
Perrin, J. Atoms 8vo, *2 50
Perrine, F. A. C. Conductors for Electrical Distribution 8vo, *3 50
Petit, G. White Lead and Zinc White Paints. 8vo, *2 oo
Petit, R. How to Build an Aeroplane 8vo, i 50
Pettit, Lieut. J. S. Graphic Processes i6mo, 075
Philbrick, P. H. Beams and Girders '. i6mo,
Phin, J. Seven Follies of Science : 12010, *r 50
Pickworth, C. N. Logarithms for Beginners .i2mo, boards, i oo
— The Slide Rule izmo, i 50
Pilcher, R. B. The Profession of Chemistry lamo (In Press.)
Pilcher, R. B., and Butler-Jones, F. What Industry Owes to Chemical
Science tamo, i 50
Plattner's Manual of Blow-pipe Analysis. Eighth Edition, revised. 8vo, 4 oo
Plympton, G. W. The Aneroid Barometer i6me, o 75
How to Become an Engineer x6oi«, o 75
Van Nostrand's Table Book i6ano, o 75
Pochet, M. L. Steam Injectors i6mo, o 75
Pocket Logarithms to Four Places i6mo, o 75
i6mo, leather, i oo
Polleyn, F. Dressings and Finishings for Textile Fabrics 8vo, *3 50
Pope, F. G. Organic Chemistry izmo, 2 50
Pope, F. L. Modern Practice of the Electric Telegraph 8vo, i 50
Popplewell, W. C. Prevention of Smoke 8v«, *3 50
Strength of Materials 8v«, *2 50
Porritt, B. D. The Chemistry of Rubber 12019, i oo
Porter, J. R. Helicopter Flying Machine . . izrno, i 50
Potts, H. E. Chemistry of the Rubber Industry 8vo, 2 50
Practical Compounding of Oils, Tallows and Grease 8v», *3 50
Pratt, A. E. The Iron Industry 8vo (hi Press.)
• The Steel Industry 8vo (In Press.)
Pratt, Jas. A. Elementary Machine Shop Practice (In Press.)
Pratt, K. Boiler Draught 12010, *i 25
Prelini, C. Earth and Rock Excavation 8vo, *3 oo
Graphical Determination of Earth Slopes 8vo, *2 oo
Tunneling. New Edition 8vo, *3 oo
Dredging. A Practical Treatise 8vo, *3 oo
Prescott, A. B., and Johnson, 0. C. Qualitative Chemical Analysis . . 8vo, 4 oo
Prescott, A. B., and Sullivan, E. C. First Book in Qualitative Chemistry.
Prideaux, E. B. R. Problems in Physical Chemistry 8vo, *2 oo
— — The Theory and Use of Indicators 8vo, 5 oo
Prince, G. T. Flow of Water iamo, *2 oo
Pull, E. Modern Steam Boilers 8vo, 5 oo
Pullen, W. W. F. Application of Graphic Methods to the Design of
i2mo, *i 50
Structures I2mo, 3 Oo
- Injectors: Theory, Construction and Working izmo, *2 oo
— Indicator Diagrams 8vo, 3 o->
— Engine Testing !ttf, *5 50
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 21
Purday, H. F. P. The Diesel Engine Design 8vo (In Press.)
Putsch, A. Gas and Coal-dust Firing 8vo, *2 50
Rafter, G. W. Mechanics of Ventilation i6mo, o 75
Potable Water i6mo, o 75
— Treatment of Septic Sewage i6mo, .v o 75
— and Baker, M. N. Sewage Disposal in the United States. .. .4to, 6 oo
Raikes, H. P. Sewage Disposal Works 8vo, *4 oo
Randau, P. Enamels and Enamelling 8vo, *s oo
Rankine, W. J. M., and Bamber, E. F. A Mechanical Text-book. .8vo, 4 oo
— Civil Engineering 8vo. 7 50
— Machinery and Millwork 8vo, 6 oo
- The Steam-engine and Other Prime Movers 8vo, 6 oo
Rankine, W. J. M., and Bamber, E. F. A Mechanical Text-book 8vo, 3 50
Raphael, F. C. Localization of Faults in Electric Light and Power Mains.
8vo, 3 50
Rasch, E. Electric Arc Phenomena 8vo, 2 oo
Rathbone, R. L. B. Simple Jewellery 8vo, 2 50
Rausenberger, F. The Theory of the Recoil Guns 8vo, *5 oo
Rautenstrauch, W* Notes on the Elements of Machine Design. 8 vo, boards, *i 50
Rautenstrauch, W., and Williams, J. T. Machine Drafting and Empirical
Design.
Part I. Machine Drafting 8vo, i 50
Part II. Empirical Design (In Preparation.)
Raymond, E. B. Alternating Current Engineering 12010, *2 50
Rayner, H. Silk Throwing and Waste Silk Spinning 8vo,
Recipes for the Color, Paint, Varnish, Oil, Soap and Drysaltery Trades,
Svo, *5 oo
Recipes for Flint Glass Making i2mo, *s oo
Redfern, J. B., and Savin, J. Bells, Telephones i6mo, o 75
Redgrove, H. S. Experimental Mensuration i2mo, i 50
Reed, S. Turbines Applied to Marine Propulsion *5 oo
Reed's Engineers' Handbook Svo, *g oo
— — Key to the Nineteenth Edition of Reed's Engineers' Handbook. .8vo, 4 oo
Useful Hints to Sea-going Engineers i2mo, 3 oo
Reid, E. E. Introduction to Research in Organic Chemistry. (In Press.}
Reinhardt, C. W. Lettering for Draftsmen, Engineers, and Students.
oblong 410, boards, i oo
Reinhardt, C. W. The Technic of Mechanical Drafting,
oblong, 4to, boards, *i oo
"Reiser, F. Hardening and Tempering of Steel i2mo, 2 50
Reiser, !N. Faults in the Manufacture of Woolen Goods Svo, 2 50
— Spinning and Weaving Calculations Svo, *$ oo
Renwick, W. G. Marble and Marble Working Svo (Reprinting.)
tteuleaux, F. The Constructor 4to, 400
Rey, Jean. The Range of Electric Searchlight Projectors Svo,
(Reprinting.}
Reynolds, ©., and Idell, F. E. Triple Expansion Engines i6mo, o 75
Rhead, G. F. Simple Structural Woodwork i2mo, *i 25
Rhead, G. W. British Pottery Marks Svo, 3 50
Rhodes, H. J. Art of Lithography Svo, 5 oo
Rice, J. M., and Johnson, W. W. A New Method of Obtaining the Differ-
ential of Functions i2mo, o 50
22 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Richards, W. A. Forging of Iron and Steel i2mo, 2 oo
Richards, W. A., and North, H. B. Manual of Cement Testing. . . . i2mo, *i 50
Richardson, J. The Modern Steam Engine 8vo, *3 50
Richardson, S. S. Magnetism and Electricity i2mo, *2 oo
Rideal, E. K. Industrial Electrometallurgy 8vo, 3 oo
— The Rare Earths and Metals 8vo (In Press.)
Rideal, S. Glue and Glue Testing 8vo, *s oo
— The Carbohydrates 8vo (In Press.)
Riesenberg, F. The Men on Deck i2mo, 3 oo
— Standard Seamanship for the Merchant Marine. i2mo (In Press.)
Rimmer, E. J. Boiler Explosions, Collapses and Mishaps 8vo, *i 75
Rings, F. Reinforced Concrete in Theory and Practice i2mo, *4 50
Reinforced Concrete Bridges 4to, *$ oo
Ripper, W. Course of Instruction in Machine Drawing folio, *6 oo
Roberts, F. C. Figure of the Earth i6mo, o 75
Roberts, J., Jr. Laboratory Work in Electrical Engineering 8vo, *2 oo
Robertson, L. S. Water-tube Boilers 8vo, 2 oo
Robinson, J. B. Architectural Composition 8vo, *2 50
Robinson, S. W. Practical Treatise on the Teeth of Wheels. .i6mo, o 75
— Railroad Economics i6mo, o 75
— Wrought Iron Bridge Members i6mo, o 75
Robson, J. H. Machine Drawing and Sketching 8vo, *2 oo
Roebling, J. A. Long and Short Span Railway Bridges folio, 25 oo
Rogers, A. A Laboratory Guide of Industrial Chemistry 8vo, 2 oo
• Elements of Industrial Chemistry i2mo, *3 oo
Manual of Industrial Chemistry 8vo, *s oo
Rogers, F. Magnetism of Iron Vessels i6mo, o 75
Rohland, P. Colloidal and Crystalloidal State of Matter i2mo,
(Reprinting.)
Rollinson, C. Alphabets Oblong, i2mo, *i oo
Rose, J. The Pattern-makers' Assistant 8vo, 2 50
• Key to Engines and Engine-running i2mo, 2 50
Rose, T. K. The Precious Metals 8vo, 2 50
Rosenhain, W. Glass Manufacture 8vo», 5 oo
— Physical. Metallurgy, An Introduction to 8vo, 4 oo
Roth, W. A. Physical Chemistry 8vo, *2 oo
Rowan, F. J. Practical Physics of the Modern Steam-boiler 8vo, *3 oo
— and Idell, F. E. Boiler Incrustation and Corrosion i6mo, o 75
Roxburgh, W. General Foundry Practice 8vo, 2 50
Ruhmer, E. Wireless Telephony 8vo, 4 50
Russell, A. Theory of Electric Cables and Networks 8vo, *3 oo
Rust, A. Practical Tables for Navigators and Aviators 8vo, 3 50
Rutley, F. Elements of Mineralogy i2mo, i 50
Sandeman, E. A. Notes on the Manufacture of Earthenware. ..i2mo, 3 50
Sanford, P. G. Nitro-explosives 8vo, *4 oo
Saunders, C. H. Handbook of Practical Mechanics i6mo, i 50
leather, 2 oo
Sayers, H. M. Brakes for Tram Cars 8vo, *i 25
Schaefer, C. T. Motor Truck Design 8vo, 250
Scheele, C. W. Chemical Essays 8vo, *2 50
Scheithauer, W. Shale Oils and Tars 8vo, *4 oo
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 23
Scherer, jR. Casein , M '. 8vo, 3 50
Schidrowitz, P. Rubber, Its Production and Industrial Uses Svo, *6 oo
Schindler, K. Iron and Steel Construction Works izmo, *2 oo
Schmall, C. N. First Course in Analytic Geometry, Plane and Solid.
i2mo, half leather, *i 75
and Shack, S. M, Elements of Plane Geometry xamo, i 25
Schwarz, E. H. L. Causal Geology Svo, *3 oo
Schmeer, L. Flow of Water 8vo, 150
Schweizer, V. Distillations of Resins Svo, 5 oo
Scott, A. H. Reinforced Concrete in Practice !2mo, 2 oo
Scott, W. W. Qualitative Analysis. A Laboratory Manual. New
Edition 3 oo
Standard Methods of Chemical Analysis Svo, *6 oo
Scribner, J. M. Engineers' and Mechanics' Companion. .i6mo, leather, i 50
Scudder, H. Electrical Conductivity and lonization Constants of
Organic Compounds Svo, *3 oo
Seamanship, Lectures on i2mo, 2 oo
Searle, A. B. Modern Brickmaking Svo (In Press,)
Cement, Concrete and Bricks , .Svo, 3 oo
Searle, G. M. "Sumners' Method." Condensed and Improved.
iGmo, o 75
Seaton, A. E. Manual of Marine Engineering Svo, 10 oo
Seaton, A. E., and Rounthwaite, H. M. Pocket-book of Marine Engi-
neering i6mo, leather, 5 oo
SeeJigmann, T., Torrilhon, G. L., and Falconnet, H. India Rubber and
Gutta Percha Svo, 6 oo
Seidell, A. Solubilities of Inorganic and Organic Substances .... Svo, 7 50
Sellew, W. H. Steel Rails 4to, *io oo
Railway Maintenance Engineering i2mo, 3 oo
Senter, G. Outlines of Physical Chemistry i2mo, *2 50
Text-book of Inorganic Chemistry i2mo, *3 oo
Sever, G. F. Electric Engineering Experiments Svo, beards, *i oo
Sever, G. F., and Townsend, F. Laboratory and Factory Tests in Elec-
trical Engineering Svo, *2 50
Sewall, C. H. Wireless Telegraphy Svo, *2 oo
Lessons in Telegraphy i2mo, *i oo
Sexton, A. H. Fuel and Refractory Materials i2mo (Reprinting.)
-Chemistry of the Materials of Engineering ismo, *3 oo
Alloys (Nan-Ferrous) Svo, 3 50
Sexton, A. H., and Primrose, J. S. G. The Metallurgy of Iron and Steel.
Svo, *6 50
Seymour, A. Modern Printing Inks Svo, 3 oo
Shaw, Henry S. H. Mechanical Integrators i6mo, o 75
Shaw, S. History of the Staffordshire Potteries Svo, 2 50
Chemistry of Compounds Used in Porcelain Manufacture. .. .Svo, *6 oo
Shaw, T. R. Driving of Machine Tools i2mo, *2 oo
Precision Grinding Machines i2mo, 5 oo
Shaw, W. N. Forecasting Weather Svo (Reprinting.)
Sheldon, S., and Hausmann, E. Dynamo Electric Machinery, A.C.
and D.C Svo (In Press.)
1 Electric Traction and Transmission Engineering .i2mo, 2 50
— Physical Laboratory Experiments, for Engineering Students. .Svo, *i 25
24 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Sherriff, F. F. Oil Merchants' Manual and Oil Trade Ready Reckoner,
Svo, 3 50
Shields, J. E. Notes on Engineering Construction i2mo, i 50
Shreve, S. H. Strength of Bridges and Roofs 8vo, 3 50
Shunk, W. F. The Field Engineer i2mo, fabrikoid, 2 50
Silverman, A., and Harvey, A. W. Laboratory Directions and Study
Questions in Inorganic Chemistry 4to, loose leaf, 2 oo
Simmons, W. H. Fats, Waxes and Essential Oils. .8vo (In Press.)
Simmons, W. H., and Appleton, H. A. Handbook of Soap Manufacture,
3/0, *4 oo
Simmons, W. H., and Mitchell, C. A. Edible Fats and Oils 8vo, *3 50
Simpson, G. The Naval Constructor i2mo, fabrikoid, *$ oo
Simpson, W. Foundations , 8vo. (In Press.}
Sinclair, A. Development of the Locomotive Engine. . .8vo, half leather, 5 oo
Sindall, R. W. Manufacture of Paper 8vo (Reprinting.)
Sindall, R. W., and Bacon, W. N. The Testing of Wood Pulp 8vo,
( Reprin ting. )
Wood and Cellulose 8vo (In Press.)
Sloane, T. O'C. Elementary Electrical Calculations i2mo, *2 oo
Smallwood, J. C. Mechanical Laboratory Methods. .. . i2mo, fabrikoid, 3 oo
Smith, C. A. M. Handbook of Testing, MATERIALS 8vo, *2 50
Smith, C. A. M., and Warren, A. G. New Steam Tables 8vo, *i 25
Smith, C. F. Practical Alternating Currents ard Testing 8vo, *3 50
Practical Testing of Dynamos and Motors 8vo, *3 oo
Smith, F. E. Handbook of General Instruction for Mechanics . . . izmo, i 50
Smith, G. C. Trinitrotoluenes and Mono- and Dinitrotoluenes, Their
Manufacture and Properties i2mo, 2 oo
Smith, H. G. Minerals and the Microscope i2mo, 2 oo
Smith, J. C. Manufacture of Paint 8vo, *5 oo
Smith, R. H. Principles of Machine Work i2mo,
Advanced Machine Work i2mo, *3 oo
Smith, W. Chemistry of Hat Manufacturing i2mo, *3 50
Snell, F. D. Calorimetric Analysis i2mo (In Press.}
Snow, W. G., and Nolan, T. Ventilation of Buildings i6mo, o 75
Soddy, F. Radioactivity 8vo (Reprinting.)
Solomon, M. Electric Lamps 8vo, 2 oo
Somerscales, A. N. Mechanics for Marine Engineers i2mo, 2 50
Mechanical and Marine Engineering Science 8vo, *$ oo
Sothern, J. W. The Marine Steam Turbine Svo, *i2 50
Verbal Notes and Sketches for Marine Engineers Svo, *i2 50
— Marine Engine Indicator Cards Svo, 4 50
Sothern, J. W., and Sothern, R. M. Simple Problems in Marine
Engineering Design i2mo,
Souster, E. G. W. Design of Factory and Industrial Buildings.. .8vo,
Southcombe, J. E. Chemistry of the Oil Industries Svo,
Soxhlet, D. H. Dyeing and Staining Marble Svo,
Spangenburg, L. Fatigue of Metals iGmo,
Specht, G. J., Hardy, A. S., McMaster, J. B., and Walling. Topographical
Surveying i5mo,
Spencer, A. S. Design of Steel-Framed Sheds Svo,
Spiegel, L. Chemical Constitution and Physiological Action. .. .i2mo,
D. VAN NOSTRAND CO'.'S SHORT TITLE CATALOG 25
Sprague, . E. H. Hydraulics i amo, 2 co
— Elements of Graphic Statics ; 8vo, 3 co
— -— Stability of Masonry i^rao, 2 oo
— Elementary Mathematics for Engineers i2mo, 2 co
— Stability of Arches i?.mo, 2 oo
— Strength of Structural Elements i2mo, 2 oo
Moving Loads by Influence Lines and Other Methods i2mo, 2 oo
Stahl, A. W. Transmission of Power i6mo,
Stahl, A. W., aad Woods, A. T. Elementary Mechanism i2mo, *2 oo
Standage, H. C. LeatherworkersP Manual 8vo, *3 50
— Sealing Waxes, Wafers, and Other Adhesives 8vo, *2 50
— AgglHtiaants of All Kinds for All Purposes i2mo, 3 50
Stanley, H. Practical Applied Physics (In Press.)
Stansbie, J. H. Iron and Steel 8vo, 2 50
Steadman, F. M. Unit Photography i2mo, *2 oo
Stecher, G. E. Cork. Its Origin and Industrial Uses i2mo, i oo
Steinheil, A., and Voit, E. Applied Optics* Vols. I. and II. 8vo,
Each, 5 oo
— . Two Volumes Set, 9 oo
Steinman, D. B. Suspension Bridges and Cantilevers. (Science Series
No. 127.) o 75
Stevens, A. B. Arithmetric of Pharmacy i2mo, i 50
Stevens, E. J. Field Telephones and Telegraphs i 20
Stevens, H. P. Paper Mill Chemist i6mo, 4 oo
Stevens, J. S. Theory of Measurements i2mo, *i 25
Stevenson, J. L. Blast-Furnace Calculations i2mo, leather, 2 50
Stewart, G. Modern Steam Traps i2mo, *i 75
Stiles, A. Tables for Field Engineers i2mo, i oo
Stodola, A. Steam Turbines 8vo, 5 oo
Stone, E. W. Elements of Radiotelegraphy i2mo, fabrikoid, 2 50
Stone, H. The Timbers of Commerce Svo, 4 oo
Stopes, M. The Study of Plant Life Svo, 2 oo
Sudborough, J. J., and James, T. C. Practical Organic Chemistry ,. lamo, 2 50
Suf fling, E. R. Treatise on the Art of Glass Painting Svo, *3 50
Sullivan, T. V., and Underwood, N. Testing and Valuation of Build-
ing and Engineering Materials (In Press.)
Sutherland, D. A. The Petroleum Industry Svo (In Press.)
Svenson, C. L. Handbook on Piping Svo, 4 oo
— Essentials «f Drafting Svo, i 75
— Mechanical and Machine Drawing and Design (In Press.)
Swan, K. Patents, Designs and Trade Marks Svo, 2 oo
Swinburne, J., Wordingham, C. H., and Martin, T. C. Electric Currents.
i6mo, o 75
Swoope, C. W. Lessons in Practical Electricity i2mo, *2 oo
Tailfer, L. Bleaching Linen and Cotton Yarn and Fabrics 3vo, 7 co
Tate, J. S. Surcharged and Different Forms of Retaining- walls. .i6mo, o 75
Taylor, F. N. Small Water Supplies i2mo, *2 50
— Masonry in Civil Engineering Svo, *2 50
Taylor, W. T. Electric Cable Transmission and Calculation. (In Press.)
Calculation of Electric Conductors 4to (In P,css.)
Templeton, W. Practical Mechanic's Workshop Companion.
i2mo, morocco, a oo
Tenney, E. H. Test Methods for Steam Power Plants i2mo, 3 oo
Terry, H. L. India Rubber and its Manrfacture. .8vo (Reprinting.)
26 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Thayer, H. R. Structural Design. 8vo.
Vol. I. Elements of Structural Design 350
Vol. II. Design of Simple Structures 4 50
Vol. III. Design of Advanced Structures (In Preparation.)
Foundations and Masonry (In Preparation.)
Thiess, J. B., and Joy, G. A. Toll Telephone Practice 8vo, *3 50
Thorn, C., and Jones, W. H. Telegraphic Connections.. . .oblong, i2mo, 150
Thomas, C. W. Paper-makers' Handbook . (In Press.)
Thomas, J. B. Strength of Ships 8vo, 2 50
Thomas, Robt. G. Applied Calculus ..izmo, 300
Thompson, A. B. Oil Fields of Russia 4to, 10 oo
— Oil Field Development 10 oo
Thompson, S. P. Dynamo Electric Machines i6mo, o 75
Thompson, W. P. Handbook of Patent Law of All Countries i6mo, i 50
Thomson, G. Modern Sanitary Engineering i2mo, *s oo
Thomson, G. S. Milk and Cream Testing i2mo, *2 25
Modern Sanitary Engineering, House Drainage, etc 8vo, *3 oo
Thornley, T. Cotton Combing Machines. 8vo, *s 50
— Cotton Waste 8vo, ^3 50
— Cotton Spinning. 8vo.
First Year *i 50
Second Year *3 50
Third Year *2 50
Thurso, J. W. Modern Turbine Practice 8vo, *4 oo
Tidy, C. Meymott. Treatment of Sewage i6mo, o 75
rilmans, J. Water Purification and Sewage Disposal 8vo, 2 50
Tinney, W. H. Gold-mining Machinery 8vo, *3 oo
Titherley, A. W. Laboratory Course of Organic Chemistry 8vo, *2 oo
Tizard, H. T. Indicators (In Press.~)
Toch, M. Chemistry and Technology of Paints 8vo, 4 50
Materials for Permanent Painting i2mo, *2 oo
Tod, J., and McGibbon, W. C. Marine Engineers' Board of Trade
Examinations 8vo, *2 oo
Todd, J., and Whall, W. B. Practical Seamanship 8vo, 12 oo
Townsend, F. Alternating Current Engineering 8vo, boards, *o 75
Townsend, J. S. lonization of Gases by Collision 8vo, *i 25
Transactions of the American Institute of Chemical Engineers, 8vo.
Vol. I. to XL, 1908-1918 8vo, each, 6 oo
Traverse Tables i6mo, o 75
Treiber, E. Foundry Machinery i2mo, 2 oo
Trinks, W. Governors and Governing of Prime Movers 8vo, 3 50
Trinks, W., and Housum, C. Shaft Governors i6mo, o 75
Trowbridge, W. P. Turbine Wheels i6mo, o 75
Tucker, J. H. A Manual of Sugar Analysis 8vo, 3 50
Turnbull, Jr., J., and Robinson, S. W. A Treatise on the Compound
Steam-engine i6mo, o 75
Turner, H. Worsted Spinners' Handbook i2mo, *3 oo
Turrill, S. M. Elementary Course in Perspective I2mo, *i 25
Twyford, H. B. Purchasing 8vo, *3 oo
Storing, Its Economic Aspects and Proper Methods 8vo, 3 50
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 27
Underbill, C. R. Solenoids, Electromagnets and Electromagnetic Wind-
ings i2mo, 3 oo
Underwood, N., and Sullivan, T. V. Chemistry and Technology of
Printing Inks 8vo, *3 oo
Urquhart, J. W. Electro-plating i2mo, 2 oo
Electrotyping , I2mo, 2 oo
Usborne, P. O. G. Design of Simple Steel Bridges 8vo, *4 oo
Vacher, F. Food Inspector's Handbook i2mo,
Van Nostrand's Chemical Annual. Fourth issue igiS.fabrikoid, i2mo, *3 oo
— Year Book of Mechanical Engineering Data (In Press.)
Van Wagenen, T. F. Manual of Hydraulic Mining i6mo, i oo
Vega, Baron Von. Logarithmic Tables 8vo, 2 50
Vincent, C. Ammonia and its Compounds. Trans, by M. J. Salter.Svo, *2 50
Vincent, C. Ammonia and its Compounds 8vo, 2 50
Virgin, R. Z. Coal Mine Management (In Press.)
Volk, C. Haulage and Winding Appliances 8vo, *4 oo
Von Georgievics, G. Chemical Technology of Textile Fibres 8vo,
—Chemistry of Dyestuffs 8vo, (New Edition in Preparation.)
Vose, G. L. Graphic Method for Solving Certain Questions in Arithmetic
and Algebra i6mo, o 75
Vosmaer, A. Ozone 8vo, *2 50
Wabner, R. Ventilation in Mines 8vo, 5 oo
Wadmore, T. M. Elementary Chemical Theory i2mo, *i 50
Wagner, E. Preserving Fruits, Vegetables, and Meat i2mo, *2 50
Wanner, H. E., and Edwards, H. W. Railway Engineering Estimates.
(In Press.)
Wagner, "J. B. Seasoning of Wood 8vo, 3 oo
Waldram, P. J. Principles of Structural Mechanics i2mo, 4 oo
Walker, F. Dynamo Building i6mo, o 75
Walker, J. Organic Chemistry for Students of Medicine 8vo, 4 oc
Walker, S. F. Steam Boilers, Engines and Turbines 8vo, 3 oo
— Refrigeration, Heating and Ventilation on Shipboard i2mo, *2 50
— — Electricity in Mining 8vo, *4 50
— Electric Wiring and Fitting 8vo, 2 50
Wallis-Tayler, A. J. Bearings and Lubrication 8vo, *i 50
Aerial or Wire Ropeways 8vo (Reprinting.)
— Preservation of Wood 8vo, 4 oo
— Refrigeration, Cold Storage and Ice Making 8vo, 5 50
— Sugar Machinery i2mo, 3 oo
Walsh, J. J. Chemistry and Physics of Mining and Mine Ventilation,
i2mo, 2 50
Wanklyn, J. A. Water Analysis i2mo, 2 oo
Wansbrough, W. D. The A B C of the Differential Calculus. .. . i2mo, *2 50
— Slide Valves i2mo, *2 oo
Waring, Jr., G. E. Sanitary Conditions i6mo, o 75
Sewerage and Land Drainage *6 oo
Modern Methods of Sewage Disposal i2mo, 2 oo
How to Drain a House i2mo, i 25
28 D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG
Warnes, A. R. Coal Tar Distillation 8vo, *5 oo
Warren, F. D. Handbook on Reinforced Concrete i2mo, *2 50
Watkins, A. Photography 8vo, 3 50
Watson, E. P. Small Engines and Boilers lamo, i 25
Watt, A. Electro-plating and Electro-refining of Metals 8vo, 5 oo
— Electro-metallurgy izmo, i oo
— Paper-Making 8vo, 3 75
Leather Manufacture 8vo, 6 oo
— The Art of Soap Making 8vo, 4 oo
Webb, H. L. Guide to the Testing of Insulated Wires and Cables. i2mo, i oo
Wegmann, Edward. Conveyance and Distribution of Water for
Water Supply 8vo, 5 oo
Weisbach, J. A Manual of Theoretical Mechanics 8vo, *6 oo
Weisbach, J., and Herrmann, G. Mechanics of Air Machinery. .. .8vo, *3 75
Wells, M. B. Steel Bridge Designing 8vo, *2 50
Wells, Robt. Ornamental Confectionery 12 mo, 3 oo
Weston, E. B. Loss of Head Due to Friction of Water in Pipes. .i2mo, 2 oo
Wheatley, 0. Ornamental Cement Work 8vo, *2 25
Whipple, S. An Elementary and Practical Treatise on Bridge Building.
8vo, 3 oo
White, C. H. Methods of Metallurgical Analysis i2mo, 2 50
White, G. F. Qualitative Chemical Analysis i2mo, 140
White, G. T. Toothed Gearing 12120, *2 oo
White, H. J. Oil Tank Steamers 121*10, i 50
Whitelaw, John. Surveying 8vo, 450
Whittaker, C. M. The Application of the Coal Tar Dyestuff s . . . 8vo, 3 oo
Widmer, E. J. Military Balloons 8vo, 3 oo
Wilcox, R. M. Cantilever Bridges i6mo, o 75
Wilda, H. Steam Turbines lamo, 2 oo
— Cranes and Hoists i2mo, 2 oo.
Wilkinson, H. D. Submarine Cable Laying and Repairing 8vo,
{Reprinting.)
Williamson, J. Surveying 8vo, *3 oo
Williamson, R. S. Practical Tables in Meteorology and Hypsometry,
4to, 2 50
Wilson, F. J., and Heilbron, I. M. Chemical Theory and Calculations.
i2mo, *i 25
Wilson, J. F. Essentials of Electrical Engineering 8vo, 2 50
Wimperis, H. E. Internal Combustion Engine 8vo, "^3 oo
Application of Power to Road Transport i2mo, ::;i 50
— Primer of Internal Combustion Engine i2mo, i 50
Winchell, N. H., and A. N. Elements of Optical Mineralogy 8vo, *3 50
Winslow, A. Stadia Surveying i6mo, o 75
Wisser, Lieut. J. P. Explosive Materials iGmo,
— Modern Gun Cotton . . . . . i6mo, o 75
Wolff, C. E. Modern Locomotive Practice 8vo, *4 20
Wood, De V. Luminiferous Aether i6mo, o 75
Wood, J. K. Chemistry of Dyeing i2mo, i oo
Worden, E. C. The Nitrocellulose Industry. Two Volumes 8vo, *io oo
— Technology of Cellulose Esters. In 10 volumes. 8vo.
Vol. VIII. Cellulose Acetate. . *5 oo
D. VAN NOSTRAND CO.'S SHORT TITLE CATALOG 29
Wren, H. Organometallic Compounds of Zinc and Magnesium, . i2mo, i oo
Wiight, A. C. Analysis of Oils and Allied Substances • 8vo, *3 50
Wright, A. C. Simple Method for Testing Painters' Materials. . .8vo, 2 50
Wright, F. W. Design of a Condensing Plant.. i2mo (Reprinting.')
Wright, H. E. Handy Book for Brewers 8vo, *6 oo
Wright, J. Testing, Fault Finding, etc., for Wiremen i6mo, o 50
Wright, T. W. Elements of Mechanics 8vo, *z 50
Wright, T. W., and Hayford, J. F. Adjustment of Observations. ..8vo, *3 oo
Wynne, W. E., and Sparagen, W. Handbook of Engineering Mathe-
matics i2ino, 2 oo
Yoder, J. H., and Wharen, G. B. Locomotive Valves and Valve Gears,
8vo, *3 oo
Young, J. E. Electrical Testing for Telegraph Engineers 8vo, *4 oo
Young, R. B. The Banket 8vo, 3 50
Youngson. Slide Valve and Valve Gears ' 8vo, 3 oo
Zahner, R. Transmission of Power i6mo,
Zeuner, A. Technical Thermodynamics. Two Volumes 8vo, 8 oo
Zimmer, G. F. Mechanical Handling and Storing of Materials. .. .4to, 15 oo
Mechanical Handling of Material and Its National Importance
During and After the War 4to, 4 oo
iZipser, J. Textile Raw Materials 8vo, 5 oo
Zur Nedden, F. Engineering Workshop Machines and Processes. .8vo, 2 oo
D. VAN NOSTRAND COMPANY
are prepared to supply, either from
their complete stock or at
short notice,
Any Technical or
Scientific Book
In addition to publishing a very large
and varied number of SCIENTIFIC AND
ENGINEERING BOOKS, D. Van Nostrand
Company have on hand the largest
assortment in the United States of such
books issued by American and foreign
publishers.
All inquiries are cheerfully and care-
fully answered and complete catalogs
sent free on request.
25 PARK PLACE NEW YORK
UNIVERSITY OF CALIFORNIA LIBRARY
BERKELEY
Return to desk from which borrowed.
This book is DUE on the last date stamped below.
280ct'49A¥
»
2iiVlayT5lUJ
2lMay54Vlf
**>
-
APR 2019
DEC 12
'
t Jan u3BP\V
REC D L
DEC 1 3 196^
i,a
LD 21-100w-9,'481B399sl6)476
<?
THE UNIVERSITY OF CALIFORNIA LIBRARY
Live Music Archive
Librivox Free Audio
Metropolitan Museum
Cleveland Museum of Art
Internet Arcade
Console Living Room
Books to Borrow
Open Library
TV News
Understanding 9/11