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i
Physici Lib.
SOLUBILITIES
OF
INORGANIC AND ORGANIC
COMPOUNDS
A COMPILATION OF QUANTITATIVE S0LUBILIT9
DATA FROM THE PERIODICAL
LITERATURE
ATHERTON SEIDELL, Ph.D.
Hysimic Laboratory, U. S. Public Heaitk
Service, Washington, D. C.
SECOND EDITION
ENLAROED AND THOROUQHLY REVISED
NEW YORK
VAN NOSTRAND COMPANY
as Park Placb
1919
Copyright, 1907, 1911, 1919,
BY
D. VAN NOSTRAND COMPANY
Stanbope pctM
F. H. GILSON COMPANY
BOSTON. U.S.A
r
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
...
m
353420
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, wUl, 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
a& those of Dan^mer, 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 Donn6es
Num^rique" 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. Pharmacopceia (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 ufee. 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-
c^y 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
vn
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),
(ft) Melting-point data for mixtures of minerals, except a few
of relatively simple composition.
• • «
Vlll
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 cbmpounds, the rules adopted
for that publication (see, in connection with index to Vol. ii,
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.
Farms 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 loo 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 instancei
xi
GENERAL INFORMATION
if It is found that loo grams of the saturated solution contain
CO 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 -5- 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
. .
xu
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 lOO 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 H2O 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
...
XiU
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 loo 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 lOO
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 ioo° contains 25 mol. per cent Hgl2,
which designates a mixture of 25 gram mols. of Hgl2 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 Hgl2 divided by the product for the QH^N. Thus,
(25 X 45445) ^ (75 X 79.08) ^ 1. 915, which, X 100, = 191. 5
grams Hgl2 per 100 grams of CcH^N.
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 (loo 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 comp)ound
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. NaNOi per 100 Cms. Mob
SoluUon. 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°, lOO
grams of the saturated solution of sodium nitrate in water contain
42.2 grams NaNOs, (2) that at 0°, 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 0° contains 6.71 gram molecules of
NaNOj.
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 sho¥ang the reslilts 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, CdIt.KI.HtO, CdIt.2KI.2H,0 and CdIt.2NaL6H,0 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 Cdlt.KI.HsO,
given in terms both of grams of anhydrous salt, Cdlt.KI, per 100
grams of solution and per 100 grams of solvent. The next group of
figures shows successively the solubility of CdIt.2KI.2HsO 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 CdIt.2NaI.6HtO.
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 difiFerent 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 bracketi
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 ^turated 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.i2H20, it will be noted that 100 grams of HjO
dissolve 106.8 grams FeCU at 30** and two lines below, the same
amount of water is stated to dissolve 201.7 grams FeCU 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.i2H20, the grams of FeCU 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.
If, 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
betw^een two inuniscible solvents (see for example, results for mer-
curic chloride, pp. 420 and 421), the amounts of the dissolved conx-
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 diiEcult 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 wiittea both wkh capitals
and without.
(all). — Specific Rotation,
abs. — Absolute.
abs. coef . — Absorption Coefficient,
aloohol. — Ethyl Alcohol.
anit(s). — AmountCs).
anhy. — Anhydrous,
aq. — Aqueous. *
atm(s). — AtmosphereCs).
at. wt. — Atomic Weight.
b.-pt. — Boiling-point.
C. — Centigrade,
calc. — Calculate(ed).
cc. — Cubic CentimeterCs).
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 (dig — Specific Gravity
at i8**, referred to water at 4**; d^
at 20* referred to water at 20**)i
decomp. — Decomposition.
dif. — Different.
dH- — Dilute.
dist. coef. — Distribution Coefficient.
ed. — Edition.
elec — Electric(al).
eqfuil. — Equilibrium. .
ec|uiv. — Equivalent(8).
eutec. — Eutcctic.
F. — Fahrenheit.
L'pt. — Freezing-point
g., gm., gms. — Gram(s).
gm. mol. — Gram Molecule(8).
G. M. — Gram Molecule(8).
hr(s). — Hour(s).
t. — {d -\- f) Inactive (in connection
with the name of an optically active
compound.)
tnorg. — Inorganic,
insol. — Insoluble.
/. — Lsevo (in connection with the
name of an optically active com*
pounid)*
kg. kgm. — Kilogram(s).
1. — Liter(8).
mm. — Millimeter (s)
m. — Meta.
max. — Maximum,
mg.y 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).
0. — 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.
8ol(s). — Solution (s).
sp. gr. — Specific Gravity (Density),
sq. cm. — Square Centimeter.
s. — Symmetrical,
sym. — Symmetrical.
ABBREVIATIONS
fc*. — Temperature, Centigrade' Scale. wt. — Weight.
teinp(s). — Temperature (s). oo — Infinity.
tr.pt. — Transition Point. .10"*, .io~*, etc, follomig 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.
x»i
▲CIMAPHTHEn
C»H
isnio*
Solubility in Several Organic Solvents.
(Spcyen — Am. J. Sd. [4] X4» 294, 1902.)
NoTB. — 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-
In Methyl Alcohol.
^ — — — ^
In Ethyl Alcohol.
— ^ ^_, —
In Propyl Alcohol.
t*.
' <a)
(*) (c) '
' (a)
(W
(0'
'(0)
(6)
(0 '
0
^^ zz
1.80 0.39
81. 1
1.9
0.57
82.3
2.26
0.88
10
80. 40
1.70 0.38
80.3
2.8
0.84
81.8
2.40
1. 00
20
79.60
2.25 0.48
79.6
4.0
1.20
81.4
340
I -35
30
79.00
350 072
79.1
5-6
1.70
80.9
4. 75
1.90
40
78 45
6.00 Z.20
78.7
8.4
2.60
80.6
7.10
2.90
50
78 IS
9.00 1.77
78.8
13.2
390
80.7
II. 10
4.40
60
78.30
11.70 2.35
79-4
23.2
7.00
81.5
19.60
8.20
70
78.60
1430 2-90
80.75
40.5
12.50
83 -9
37.00
16.20
t •.
In Chloraform.
In Toluene.
(a) (*)
(0'
'(a)
W
kcS
0
143.8 16
.4 12.7
90.7
13 18
19
10
140 . I 20
.6 16.0
90.8
18.0
10.7
20
136.3 27
.0 19.5
91.0
245
145
30
132-4 34
0 25.0
91.8
US
20.5
40
128.0 42.5 32.0
92.7
47 0
28.0
SO
123-4 V-
5 400
94 0
60.5
35-7
60
119. 3 62
s 500
95 S
74 0
43 S
70
•
• . • • 4
. ■ • •
97.2
89.0
52.5
ijA Wciglit of 100 cc. solution in gtBias. (ft) Grams dissolved sabstance per xoo grams solvent.
(c> Gfam molfnilw of dissolved substance per xoo gram molecules of solvent.
ipoo gms. Aq. 25% NHs dissolve 0.07 gm, acenaphthene at 25^. (Hilpert, 1916) .
RBdFKOCAL SOLUBILITIBS DbTERMINED BY THB METHOD OF LOWERING OF THE
Frkezing-point * Are Given by Giua (191 5), for the Following Pairs
OF Compounds:
Acenaphthene + m Dinitrobenzene.
+ 2.4 Dinitrotoluene*
+ a Trinitrotoluene.
II
<i
* Pfweaimg or Mdting-point Curves as SoMfiliiy Data. ~ When a mixture of two oompoonds, rendered
by elevation of temperature, is gradually cooled, a point will be reached at which one or the other
of the ooDstituents wfll separate as a solid. This point represents the solubility of the one compound in
the other. The method involved, differs principality from that ordinarily employed for solubility de-
tenninatioos, in that the composition of the mixture remains constant while the saturation tezbpera-
tuve B being approached, instead of the reverse procedure.
A considerable amount of data of this character is available, but, after careful consideration, it has
been drrMV^ that references only will be given to it in the present volume, except in cases of mixtures
cl veO-known oompoonds or of those in which water is one ol the constituents.
ACINAPHTHENE
Reciprocal Solubilities (Freezing-point Lowering Data, see footnote, page i)
Are Given for the Following Pairs of Compounds:
Aoenaphthene + Chloroacenaphthc
" 4" Bromoacenaphth<
lene
lene
+ lodoacenaphthene
4- Benzil
4- p Nitrobenzoic Aldehyde
4- Piperonilic Aldehyde
4- Vanillic Aldehyde
Chloroacenaphthene + Bromoacenaphthene
" " + lodoacenaphthene
Bromoacenaphthene +
(CrampCon ud Walker, zgza.)
•<
•<
M
M
«
(PawkwBki, 1893.)
(Faa, 19x6.)
tt
u
(Crompton ud Walker, 19x9.)
11
It
u
(I
II
ACETALDEHTDE CH<COH.
Solubility in Ethyl Alcohol Determined by the Method of Lowering
OF Freezing-point (de Leeuw, 191 1). Liquid air was used as the cooling
medium and temperatures were measured with the aid of a specially con-
structed resistance thermometer.
wt.
Mol.
Wt.
Mol.
Per Cent
Per Cent
Per Cent
Per Cent
f.
CHjCOH CHjCOH
Solid Phase.
r.
CH,COH CH,COH Solid Phase.
in
in
in
in
Mixtuxe.
Mixture.
Mixture.
Mixture.
123.3
100
100
CHiCOH
— 122.3
51.8
50.7 CHjCOH-CHdOH
125.4
90.7
90.3
«
-125.3
45.6
44
5
127.6
84.5
83.9
fi
-128
40.6*
39
.5 CH,C0H.2CrfV)H
132
80.9
80.2
(Eutectic)
—123.2.
35.3
34
3
126
78.1
77.3 C^|COH.C,H^H
-126.8
30.2
29
3
126
75.2
74.4
<i
—130.6
17.9
17
.3 CAQH
124.3
67.0
66.0
II
— 120.6
10.2
9
.8
123. 5
60.8
59-7
II
-114. 9
0.0
0
.0
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 Patemo and Ampola (1897).
Results for mixtures of the a and fi forms of Acetaldehyde phenyl hydrazone
are given by Laws and Sidgwick (191 1).
AOETAMIDE CH,CO.NH,.
Solubility in Water and in Alcohol.
(Speyers.)
In Water.
In Ethyl Alco
' (a) (4)
hoi.
%•.
' (a)
(«
(0 '
(0'
0
105 S
70.8
29.6
85.62
17-3
18.5
10
104.9
81.0
34 0
86.2
24.0
26.0
20
104.3
97-5
40.8
87 -3
315
33-8
30
103.7
1140
47-7
88.8
40.5
43 0
40
103.0
133 0
55 S
90 7
50. 0
53 S
so
102.3
154.0
64.0
93 0
61.0
64 5
60
IOI.6
177s
740
95 S
72.0
76.5
' (a) Wt. of xoo cc. sat. solution in gms. (6) Gms. Acetamide per xoo gms. solvent, (c) Gm. mob.
Acetamide per xoo gm. mols. solvent.
100 gms^ pyridine dissolve 17.75 S^s. acetamide at 20-^5^; 100 gms. aq. 50 per
cent pjnidine dissolve 84.7 gms. acetamide at 20-25°. (Dehn, 1917.)
Freezing-point curves are eiven for: Acetamide + Benzene (Moles and
Jimeno, 1913); Acetamide + Phthalide (Lautz, 19 13); Acetamide 4- Triphenyl
guanidine (Lautz, 19 13); Tribromoacetamide -h Trichloroacetamide (Kttster,
1891).
ACITANILZDB
ACBTANIUDE
C«H»NH.COCH,.
S(M.UBiLiTY IN Several Solvents.
Solvent.
r.
Sp. Gr.
of Sat.
Solution.
Gms.
QH,NH.C0CH|
per 100 Gms.
Sat. Solution.
Authority.
Water
16
• « •
0 . 47 (Greenish and Smith, 1903.)
<(
25
0.997
0 . 54 (HoUemanand Antush, 1894.)
((
30
1. 000
0.69
(SeideU, 1907.)
Ether
25
...
2.8 CHaiden and Dover. 1916.)
Formic Add (95%)
16. 8" 1. 121
56.74
Acetic Acid (99.5%}
21.
s
33-21
(Seidell. 1907.)
Acetone
30-31 0.902
31 15
M
Amyl Acetate
«
0.882
10.46
M
Amyl Alcohol
25
• • •
14.00
M
Aniline
30-31 1 .034
19.38
M
Benzene
u
0.875
2.46
M
Benzaldehyde
It
1.068
18.83
M
Toluene
25
0.862
0.50
M
Xylene
32.
5 0-847
1.65
l(
Pyridine
20-25
32.7
(Dehn, 19x7.)
56% Aq. Pyridine
u
...
35.7
II
Petroleum Ether about
20
0.03
(Salkower. 19x6.)
SoLUBn-mr in
r Methyl Alcohol, Ethyl Alcohol and
IN CmxmoFORM.
(Speyexs, 1902.) See Note, page i.
In CHdOH.
In CH^H.
In CHCV
sp. Gr. of
f . Sat. Sdu-
tkm.
Gms.
C,H|NH.COCH.
per 100 Gms.
Sat. Solution.
*^*^ St. Solution. ^"°^
CANHOOCH.
per 100 Gnm.
Sio. Sedation.
0 C.860
18. s
0.842
12.8 I
.503
3-53
10, 0.864
23.1
0.844
16.7 I
•475
7.34
20 •' 0.87s
29.1
0.850
21.3 I
.440
10.7
30 0.892
35.1
0.860
26.5 I
.398
14.5
40 O.9II
42.9
0.874
32.9 I
.354
18.7
50 0.932
Si-7
0.895
39.4 I
•314
237
60 0.957
59-2
0.920
46.4 I
.272
29.x
SoLUBiLrrr of ^
^CETANILmE IN MIXTURES <
DF Ethyl Alcohol
AND Water.
^^ Results at 25*. (HoUeman and Antuah, 1894.)
Results at
30*. (Scidcn. 1907 )
rerOeot ^
ClUfOH in Sp. Gr. of Sat.
Sohrent. Solution.
Gms. C«HtNH.COcd»
per 100 Gms. Sat.
Solution.
Sp. Gr. of Sat.
Solution.
Gms. CANHXX)ai«
per 100 Gms. Sat.
Solution.
0 0
•997
0.54
1. 000
0.69
10 0
.985
0-93
0.984
I.QO
20 0
•973
1.28
0.970
2.20
30 0
.02
2.30
0.956
4.80
40 0
•950
4.85
0-945
'9.40
SO 0
•939
8.87
0.934
1540
60 0
.928
14.17
0.926
22.00
70 0
.918
19.84
0.917
27.60
80 0
.907
25.17
0.907
31.20
8s 0
.899
26.93
0.900
3170
90 0
.890
27.65
0.893
31-60
95 0
.874
26.82
0.885
30.80
100 0
.851
24.77
0.870
99.00
(See remarks under a Acetnaphthafide, page 13.)
ACETAMILIDE 4
Solubility of Acetanilidb in Mixtures op Ethbr and Chloroform and of
Acetone and Benzene at 25"*. (Marden and Dover, 1916.)
Results for Ether-Chloroform Mixtures. Results' for Acetone-Benzene Mixture.
'f*-£?S'Si^^?'' ^.S^Mtod" vtjyc«tcA ^^.S^Stod*
in Mixed Solvent. *^ SohJwttl. ^^ "* Mixed Solvent. '^ SohrenL ^^
100 17.7 100 1.36
90 II. 7 90 6.78
80 8.2 80 13.0
70 6.2 70 20.0
60 4.95 60 29.2
SO 4-25 SO 30 o
40 3S 40 30.5
30 35 30 330
20 3.25 20 36.0
10 3 OS 10 45.7
o 2.9 o 39.4
Distribution of Acetanilide between Immiscible Solvents at 25^.
Cone CeHsNH.COCHi in Benzene layer -j- Cone, in HiO layer — 1.65.
(Farmer and Warth, 1904.)
" " " Chloroform " •*- Cone, in HiO layer = 7.75.
(Marden, 1914.)
" Ether " 4- Cone, in H,0 layer = 2.98.
(Mardoi, 19x4.)
Solubility of Halogen Substituted Acetanilides in Ethyl Alcohol at
Different Temperatures. (Chatuway and Lambert, 19x5)
Gm^. of Each Anilide per xoo Gms. of Each Sat. Solution.
f.
r
^Chloro-
2.4Dichk>fo-
^Bromo-
9.4 Dibromo-
4Chloro-
2 Chloro-
4 Bromo-
acetanilide.
aoetsnilide.
aoetanilide.
acetanilide.
aoetanilide.
2 J3iuiu<^
acetanilide.
5
4.244
2.480
• • •
...
10
3 278
3.o<i8
4.847
2.876
4.334
2.S7S
IS
3-777
3 564
SS6i
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
4.09s
30
5.828
5,864
8.440
5.615
8.328
4.891
35
6.700
6-937
9-715
6.686
9.844
5.820
40
7.728
8.276
II. 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 bromoaeetanilide and 2.4 dibromo-
aeetanilide are also given.)
Solubility of p Nitroacetanilide and of 2.4 Dichloroacetanilide in
Acetic Acid at I6^ (Orton and King, 191 x)
CO""-""- Solvit. °^,S??2:E»*
p Nitroacetanilide Glacial Acetic Acid 0.83
So%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 (Coroanduccl. 19x2.)
" " tn Nltraniline (Crompton and Whitdey, 1895.)
m Dinitrobenzene " "
« Dinitrophenol " **
p Nitroacetanilide (KOster, x89x.)
P Nitroacetanilide and Dinitroacetanilide (Holleman and Sluiter, 1906.)
p Bromoaeetanilide and 24 Dibromoaeetanilide (Sidgwick, X9X5.)
it
u
«
II
u
II
ACETIC ACID
ACETIC ACID CHiCOOH.
Reciprocal Solubility of Acetic Acid and Water Determined by the
Method of Lowering of the Freezing-point.
GiiM.CHtCOOH
Gm. CHjCOOH
f.
per 100 Gms.
SoL Sohition.
Solid Phase.
V.
per xoo Gms.
Sot. Solution.
SoUd Phase.
o
0
Ice
— 20
67.0
CHgCOOH
- S
15.2
-IS
72.3
— ID
28. s
— 10
77-5
-IS
40.0
- s
82.2
— 20
49.2
0
87.0
-2S
57. 0
+ 5
91.8
-26.
7 60.0
(Eutectic)
10
95-8
-25
62.5
CHjCOOH
16.6
100. 0
The data in the above table were obtained by plotting the results of Pickering
(1893), Roloff (1895), Dahms (1896) (1809), deCoppet (1899), Kremann (1907),
Faucon (1910), Ball6 (1910), Groschuff (191 1), Patemo 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, BaI16 also analyzed the sofid 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.)
-75
Cms. CH,C00H
per zoo Gms.
Sat. Solution.
26.0
Solid Phase.
CHaCOOH
f.
— 10
Gms. CHiCOOH
per zoo Gms.
SeX. Solution.
67.7
Solid Phase.
CHaCOOH
-70
-60
-SO
27.7
33 0
38.2
- 5
0
+ 5
73-2
79.1
85.2
m
-40
-30
— 20
43.7
50.2
58.0
10
IS
16.6
915
98.0
100. 0
(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 Add
and Each of the Following Compounds:
Chloroacetic Acid (Mamell and Mannessier. Dimethylpyrone (Kendall, X9Z4 (a).)
1913; Kendall. z9Z4.) Dimethyl Oxalate (Kendall and Booge, 1916.)
Dichloroacetic Acid (Kendall, i9r4.) Dimethyl Succinate (Kendall and Booge, Z916.)
Tnchloroacetic Acid (KendaU. 1914.) Ethyl Ether (Pickering. Z893.)
Acetic Anhydride (Pickering, 1893.) Ethylene Bromide (Dahms.i89s; Baud. i9»(a).)
Benzene (Dahim. if9S, 1896; »<*>«, z89s; Gm^ Ethylene Dibromide (Baud. 1912 (6).)
chuff, i9zz; Baud, 1912, I9Z2 (a); Kendall and _, -^ .• , ... , «,
Booge. i9z6.)
Benzene + Vaseline (Rok>ff. 1895.)
Benzene + Naphthalene (Robff, 1895.)
Benzene + Water (Roloff. 1895.)
Benzene Acid (Kendall. 19x4.)
Chlorobenzene (Band. 1913 (c).)
Nitrobenzene (Dahms. 1895; Baud, 19x3 (c).)
Carbon Disulfide (Pickering, z893.)
Cydohexane (Baud. 1913 («) ih).)
Formamide (English and Turner, Z9Z5.)
Formic Acid (Baud, 1913 (0)
Methyl Alcohol (Pickering, 1893.)
Picric Acid (Kendall, i9z6.)
Propyl Alcohol (Pickering, Z893.)
Sulfuric Acid (Pickering, Z893.)
Thymol (Patemo and AmpoUt, Z897.)
p Xylene (Patemo and Ampola. 1897.)
ACETIC ACm
Distribution of Acetic Acm between:
Water and Amyl Alcohol
at 20^
Water and Benzene a1
:25^
(Hers and Fischer, 1904.)
(Hen and Fischer. 1905.)
Gms. CHsCOOH
G. M. CHjCOOH
Gms. CHsCOOH
G.M.<
CHtCOOH
per 100 cc.
per
xoo cc.
per
100 cc.
per
100 cc.
H9O Almholic
HjO
Alo^olic
biO
CeH.
'HsO
COIe
Layer. Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
I 0923
001
00095
5
0.130
0.05
0.0014
2 Z .847
003
0.0280
10
0.417
010
0.0005
3 2.741
0.05
0.0460
20
1-55
0.20
00030
4 3 694
0.07
0.0645
30
3 03
0.30
00290
5 4.587
0.09
0.0830
40
4-95
0.50
0.051
6 5-475
CII
OIOIO
• •
• • •
0.70
0.090
7 6.434
0.13
01190
8 7.328
• • •
• • •
Note. — The distribution results of Herz and co-workers are reported in
millimolecules per 10 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.
CWaddell, 1898; see also Lincohi, 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
•
*•.
CtigCOOH.
QH..
H26.
dlsCOO£
[. CeHe.
H2O.
25
0.46
99 52
0.02
9.4
0.18
90.42
25
3.10
96.75
0.15
28.2
053
71.27
25
5.20
94-55
0.25
37.7
0.84
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
305
67 -37
2.13
66.0
13.8
20. 2
25
52.5
39.60
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
033
36.8
1.42
62.78
35
9.0
90.42
0.58
49 0
2.10
48.90
35
45 0
49.00
6.0
61.3
255
^3'^
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 ACm
DlSTSIBDTION OF ACBTIC ACID BETWEBN WATER AND CHLOROFORM:
At Room Temperature. At 25**.
(W!rigfat, ThomKm and Leon — Pnc. R^y. (Hexx and Lewy; Rothmnnd and Wilamoire.)
Soc.49bx85«z89i0
Resahs in ports per zoo ports of solution.
Upper Layer. Lower Layer.
Gma. CHiCOOH
per 100 cc.
Ca^OOH. CHOa. HjO. CHtCOOH. CHQa. H3O.
G. M. CBsCOOB
per 100 cc.
O
6.46
17.69
25.10
33 71
44.12
50.18
0.84
0.92
0,79
1. 21
2.97
7-30
15. II
99.16
92.62
81.52
73 69
63 32
48.58
34.71
o
1.04
383
6.77
11. 05
17.72
2S-7S
99.01 0.99
98.24 0.72
94.98 I. 19
91.85 1.38
87.82 I. 13
80.00 2.28
70.13 4.12
HsO
Layer.
2
4
6
8
10
12
20
30
40
SO
52-3
CHCl,
Layer.
0.089
0.313
0-595
0.974
1.430
1.982
5.10
10.2
^5-3
21.9
39-54
HsO CHCU
Layer. Layer.
0.05 0.0032
0.075 0.0062
O.IOO O.OIOO
0.150 0.0198
0.175 0.0260
0.200 0.0325
0.30
0.50
0.70
0.80
0.87
0.070
0.170
0.275
0-335
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
add between water and chloroform are given by Rothmund and Wilsmore and
by Dawson and Grants
Distribution op Acbtic Acid at 25** between:
Water and Carbon Bisulphide.
(Hen and Lewy.)
Water and Carbon Tetrachloride
(Hers and Lewy.)
Gms. CH^OOH
G. M. CHtCOOH
Gms. CH^OOH
G.M.
CHsCOOH
per
SCO cc.
per xoo cc.
per
zoo cc.
per 100 cc.
'HiO
cs.
HiO CSi'
H,0
ecu
HiO
ecu
Layer.
Layer.
Layer. Layer.
Layer.
Layer.
Layer.
Layer.
6s
2.64
I.I 0.45
30
1.8
o-S
003
70
30
1-2 0.55
40
30
0.7
o-oss
75
3-3
1.2 0.80
so
4.8
0.9
0095
80
S-4
1-35 0-97
60
S-8
I.I
OIS5
8S
6.4
1.4 1.3
70
12.0
1.2
0'^35
76.3
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
fay Herz and Kurzer (i9io)»
Distribution op Acetic Acid at 25° between:
Water and Bromoform.
(H. and L. ~ Z. electro. Ch. 11, 8z^ '05.)
Water and Toluene.
(H. and F. — Ber. 38, 1x40, '05.)
Sms. CHaCOOH
Q. M. C:HsCOOH
Gms. CHsCOOH
G.M.
CHsCOOH
per 100 cc.
per 100 cc.
per 100 cc.
per 100 cc.
HK> CHBrs
Layer. Layer.
HaO
Layer.
CHR^
Layer.
H2O C*H«CH,
Layer. Layer.
'H2O
Layer.
C^aCHs
Layer.
ao 1.5
0.4
0035
5 0.119
O.I
0.0025
30 30
0.6
0.070
10 0.328
0.2
0.0075
40 4.8
0.8
0.120
20 1 . 132
0.4
0.0260
SO 7-8
I.O
0.20
30 2 . 265
0.6
0.0530
60 12.0
I.I
0.28
40 3- 72s
0.8
0.090
65 15.6
IIS
0.39s
50 5.841
1.0
0.140
70 27.0
• . •
...
60 8.344
• • •
• • •
See Note, page 6b
ACETIC ACID
8
Distribution of Acetic Acm between Water and Ethtl Ether.
(de Kolooaovsky, 19x1.)
Results at Several Temperatures.
Results at i8^
Cms. CBiCXX>H
per 100 cc. of:
P
Gnu. CHsCOGH
per 100 cc. of:
Ether
f.
w>
Ether
P
LiyerC^).
Layer (pO-
?'
Layer (^).
Layer (^0-
r
13
0.365
0.207
1.76
i.o
0.5
2.0
18
0.367
0.201
1.82
2.0
1.0
2.0
27
0.375
0.19s
1.94
4.0
2.1
1.9
75
0.799
0.551
1-45
6.0
3.5
1-7
12
0.803
0.529
1.52
8.0
4.9
1.6
18
0.802
0.501
1.60
10. 0
6.6
1-5
25
0.789
0.474
1.66
150
20.0
11.4
17.0
1-3
1.2
•
25.0
23 -3
1.07
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 HsO 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 CaCl2.6HsO
and ether and molten LiN0s3H|0 are given by Morgan and Benson (1907).
One determination of the distribution of acetic acid between sat. aq. CaCU
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 op Acetic
Water and o or p Xylene.
(Herz and Fischer.)
G. M. CHaCOOH
per 100 cc.
Acid at 25° between:
Water and m Xylene.
(Herz and Fischer.)
Gma. CHsCOOH
per 100 cc.
HsO
Layer.
5
10
20
30
40
SO
60
70
o or p
Xylene
Layer.
024
048
I
2
3
5
7
13
IS
40
10
27
HsO
Layer.
01
0.2
0.4
•0.6
0.8
1.0
1.2
O OT P
Xylene
Layer.
0.004
0010
0.025
047
079
122
230
O
O
o
o
12.52
See Note, page 6.
Gms. CHsCOOH
per 100 cc.
HsO
AM
5
10
20
30
40
50
60
006
0.30
095
1. 91
3 -04
4-65
6.65
G. M. CHsCOOH
per 100 cc.
HsO
Layer.
9.1
0.2
0.4
0.6
08
1.0
1.3
m
Xylene
Layer.
0.0015
0.007
0.022
0.042
0.07a
O.III
• • •
Data showing effect of camphor on the reciprocal solubility of acetic acid and
olive oil are given by Wingard, 191 7.
ChloroAGBTIC AGID8
ChloraAGBTIC ACID8 CHiQCOOH, CHOsCOOH, and CCUCOOH.
SOLUBIUTT OP THE or, /3, AND y MODIFICATION OF MONOCHLOROACBTIC ACID
IN Water at Different Temperatures.
CMiera and Isaac, 1908; Pickeriog, 1895.)
The determinations were made by the sealed tube method. The following
gure
s were obi
tamed Dy
piotung tn
e ongmai results 0
Q cross-a
action paper:
GflB.per
xoo Gms. of Eacb Sat.
Gms. per xoo Gms. of Each Sat
Solutioa.
t»
Solution.
r.
« Mpdifi-
^Modifi-
YModifi.
ttModift.
^Modift.
rModifi.
cation.
cation.
w •
cation.
cation.
cation.
20
• • •
a • •
88.0
S^,
9SO
97.0
99.6
25
• • •
85.8
90.0
SI (m. pt.)
• • •
. ../
zoo.o
30
86.0
88.2
92.2
ss ,
97.8
99-3
• • •
35
88.4
90.6
94.1
56 . s (m. pt)
• ■ •
too.o
• • •
40
90.8
93 0
95.8
60
99.0
• • •
• • •
45
93 0
95 0.
97.8
62.4 (m. pt.)
TOO.O
• • •
• • •
Reciprocal solubilities of mono-, di-, and trichloroacetic acids and water de-
termined by the freezing-point method are given by Pickering (1895).
SOLUBILITT OF TrICHLQBOACBTIC ACID IN WaTBR AT 25^
(SddeU, 1910.)
100 gms. saturated solution of ia *- 1.615 contain 92.32 gms. CClt.COOH.
SoLUBiLXTT Data Determined by the Method of Lowering of the Freez-
ing-point (see footnote, page i) Are Given for Mixtures of Chloro-
acetic Add and Each of the Following Compounds:
Dichloroacetic Add (Kendall, 19x4.)
Trichloroacetic Acid (Kendall, 19x4-)
Aoetophen<Mie (Kendall and Gibbons, x9xs.)
Dibenzyl Acetone (Kendall and Gibbons, X9XS.)
Benzil (Kendall and Gibbons, x9x5.)
Benzene (Kendall and BooBc, x9x6.)
Benzoic Acid (Kendall, X9X4.)
Camphor (Pawlewaki, 1893-)
Cinnamic Add (Kendall, X9X4.)
Crotonic Add
Cetyl Alcohol (Mamdi and Mannrsiiier, X913.)
0 Cresol (Kendall, X914.)
Methyl Cinnamate (Kendall and Booge, 19x6).
Dimethyl Oxalate (Kendall and Booge, X9x6.)
Dimethyl Succinate (Kendalland Booge, 19x6.)
Dimethylpyrone (Kendall, x9X4 (a).)
Naphthalene (Mien & Isaac, 1908; M. ft M.,X9i3.)
Phenol (Kendall, 1916.)
Piperonal (Kendall ^Gibbons, 19x5; M.&M.,X9X3.)
Salol (Mameli and Manneasier, X9X3.)
Sulfuric Acid (Kendall and Caipenter, X9X4.)
0 Toluic Add (Kendall, X9X4.)
m
P
a
II
II
II
II
II
u
u
M
Vanillin (Kendall and Gibbons, X9X5.)
SoLUBiLiTT Data Determined bt 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
0 Toluic Acid
Benzoic Add
Cinnamic Add
p " "
Crotonic Add
Dimethylpyrone
(Phenylacetic Acid)
ChloroAOITIC ACID
10
Solubility Data Dbtbrionbd bt thb Metbod of Lowbbing op thb FsBsa^
iNG-PoiNT (see footnote, page i) Are Given for Mixtures of Trichloro-
aeotlo Acid and Each of the Following Compoundf:
Acetophenone (KeiuUU and Gibbom, 19x5.)
Anisaldehyde
Benzene (Kendall and Booge, 19x6.)
Benzaldehyde (Kendall and Gibbons, x9Z5-)
m Hydroxy Benzaldehyde
p " " «
0 Nitro Benzaldehyde
^^ II II
fn
J. II «
(Elendall and
Gibbons,
Z9XS)
Benzophenone
Benzil
Benzoquinone
Benzoic Acid (KendaU, 1914)
Camphene (Timoleiew & KzavtBOV, 1915, 1917.)
Cinnamic Acid (Kendall, 1914.)
Crotonic Add
0 Cresol (Kendall, 19x4.)
fn
Diethyl Oxalate (Kendall and Boo^e, 19x6.)
Diethyl Succinate
Dimethyl Oxalate
Dimethyl Malonate "
Dimethyl Succinate
Dimethyl Terephthalate (Kendall and
BoQge. 19x6.)
Dimethylpyrone (Plotnikov, x9xx; Kendall,
X9X4 la).)
••
•c
*•
««
•I
••
Ethyl Ether CTsakalotos and Gajre, x9xa)
Ethyl Acetate (Kendall and Booge, X916.)
Ethyl Benzoate
Methyl Benzoate
" Anisate
" Cinnamate
" pToluate
a Naphthol (Kendall, X9z6.)
a Naphthyl Acetate(Kcndall and Booge, 1916.)
O (t « II u
Phenol (Kendall, X9x6.)
o Nitro Phenol (Kendall, 19x6.)
«aa II II (I
p " "
Piperonal (Kendall and Gibbons, Z9zs^
Nitro Piperonal
Phenyl Anisylketone "
" Benzoate (Kendall and Booge, I9z60
" Salicylate
Salicylic Aldehyde(Kendall and Gibbon8,z9i5>)
Sulfuric Add (Kendall and Carpenter, I9Z4-)
0 Toluic Add (Kendall, 19x4.)
tn " " "
p
a
Thymol (KendaU, 19x6.)
Vanillin (Kendall and Gibbons, 1915^
II
4<
tt
Distribution of Chloracetic Acid between:
(Hen and Fischer.)
Water and Benzene at 25°.
G. M. CHsClCOOH
Water and Toluene at 25®.
Gms. CHaQCOOH
per xoo cc.
£0
Layer.
0.35*
0.5
I.O
2.0
30
40
Layer.
8.69
IS 59
37.87
41-10
Sa-90
68.01
76.53
per zoo cc.
HsO
Layer.
0.0025
0.005
O.OIO
0.015
o.oa
0.03
0.04
C.H.
Layer.
Gms. CHiaCOOH
per 100 cc.
Layer.
0.090 O.I
0.155 0.5
0.28 1.0
0.415 i-S
054 2.0
0.70 3.0
0.79 4.0
5.0
* See Note, page 6.
CoHftCfia
Layer.
5.22
20.31
34 87
4914
60.46
72.28
81.72
86.94
G. M. CHsaCOOH
per 100 cc.
CjIUCH,
5o~
Layer.
O.OOI
0.005
O.OIO
0.015
0.02
0.03
0.04
0.05
Layer.
0.055
0.20
0.36
0.50
0.62
0.77
0.85
0.90
Additional data for the distribution of monochloroacetic acid between water
and benzene as well as similar results for dichloroacetic add are given by
Georgievics, 1915.
OiloroACETIC ACIDS
DisnaBunoN of Chloracetic Acid between:
(Hen and Lewy.)
c.
"Water and Chloroform at 25**. Water and Bromoform at 25**.
ma. rnHaClCOOB
per 100 cc«
G. M. CHtaCOOH
per 100 cc
Gou. CHiaCOOH
per xoo oc.
G. M. CH^COOH
per 100 cc
Layer.
CHOi
Layer.
CHOi ■
Layer.
Layer.
CHBu
Layer.
Layer.
Layer.
s*
XO
ao
0.283
0.614
1.088
0.05
O.IO
0.20
0.0025
0.0060
0.0135
40*
SO
60
0.850
Z.889
2.994
0.45
0.50
0.60
O.OII
0.0165
0.028
40
SO
60
70
2.948
3.684
4.440
7.086
0.40
0.60
0.70
0.7s
0.029
0.045
o.o6z
0.077
70
80
90
. 91 .6
4.241
5.620
7.560
11.340
0.70
0.80
0.90
0.97
0.040
0.053
0.067
0.120
DisTUBimoN OF Chlosacetic Acid between:
(Hen and Lewy.)
Water and Carbon Disulphide
at 25^
Wat^ and Carbon Tetra-
chloride at 25^.
Oma. CHdClCOOH
per xoo oc.
G. M. CHiQCOOH
per xoo cc.
(Sms. CHtClCOOH
per 190 cc.
G. M. CHiaC(X>H
per xoo oc.
^H*0 CS.
Layer. Layer.
Layer.
csi
Layer.
HjO ecu
Layer. Layer.
HsO
Layer.
ecu
Layer.
(So* 0.426
0.6
0.0042
90* 1. 417
0.9s
0.015c
80 0.691
0.8
0.007
95 2.031
1. 00
00195
90 0.803
I.O
0.009
100 2.645
X.05
0.0270
100 1.040
1. 05
0.0105
105 4.26
I.IO
0-0415
105 I .464
X06.7 X.890
I.IO
1. 13
0.015
0.020
* See Note
106,7 5.19
.page 6.
1. 13
0.0550
Results showing the influence of sulfuric acid upon the distribution of mono-
chlcMDacetic add between water and ethyl ether at 26"* are given by Hantzsch
and Vagt (i90i).
CyanoACXTIC ACID CH,(CN)C(X)H.
Distribution of Cyanoacbtic Acid bbtwbbn:
(Haotach and Sebalt, 1899.)
Water and Ethyl Ether.
Gms. CB^CN)C00H per
Water and Benzene.
Gma. CH|(CN)C(X)H per
Liter.
•r.
H^
Layer.
' Layer.
» .
Layer.
CJEU '
Layer.
0
10
ax
30
0.070
0.076
0.083
0.089
0.042
0.044
0.030
0.027
6
as
0.067
0.130
0.020
0.019
PhenylACBTIC ACID
13
PhenylACETIC ACID (a Toluic Add) CHs(C«Hi)COOH.
Solubility in Water and in Alcohols. (Tunofdew, 1894.)
Solvent.
r.
Gms.CHt(C«H|)COOH
Water 20
Methyl Alcohol —17
-13
((
u
Ethyl Alcohol
«
o
+ 194
20
-17
-13
per 100 Gnu.
Sat. Sol.
1.64
50.6
53-2
59-2
70.8
71.8
39-7
41. S
SdvenL
Ethyl Alcohol
Gnu. CHtCCH^COOH
t*. per 100 Gms.
Sat. SoL
0.0 50.7
+ 19.4 64.4
20.0 65.1
Propyl Alcohol —17.0 29.4
-130 32.3
0.0 40.9
+19.4 56.8
20.0 57.2
«
((
((
it
tt
(t
Solubility of Phbnylacetic Acid in Several Solvents at 25*.
(Hers and Rathmann, 1913.)
Gms. Gms.
Solvent. CHt(CA)C00H Solvent. CHs(CA)CXX>H
per 100 cc. Sat. SoL per xoo oc Sat. SoL
Chloroform 60.17 Tetrachlorethylene 21.19
Carbon Tetrachloride 25.07 Tetrachlorethane 61.45
Trichlorethylene 44 89 Pentachlorethane 44.26
The freezing-point cur^e (Solubility, see footnote, page i) is given by Sal-
kowski (1885) for mixtures of phenylacetic add and hyarodnnamic add.
ACETIC ACm ESTERS.
Solubilities of Several Acetic Acid Esters in Aqueous Alcohol at Room
Temperature. (Pfeiffer, xSga.)
oc H^ added to cause separation of a second phase in miztuies of the given
amounts of Alcohol and 3 oc. of:
r- * »
CHiCOOCH^ CH,C00CiH«. CHiCOOCtHi. CHiCOOQH^ CHiCOOQHu'
00
cc. Ethyl
Alcohol in
Mixtures.
3
6
9
12
IS
18
21
24
27
30
33
ChloroACETIC ACID ESTEBS.
Solubility of Monochlor, Dichlor, and of Trichloracetic Ester
in Aqueous Alcohol at Room Temperature. .
{Bancroft — Phys. Rev. 3, 193. 1895-96. from results of Pfeiffer. Z. physik. chem. 9p 469» ^^
6.0
4.50
2.08
1.76
00
10.48
6.08
4.24
17.80
10.46
9-03
26.00
1537
13.24
35-63
20.42
17.52
47 so
26.60
22.22
58.71
31.49
26.99
00
37.48
32.14
• • •
43.75
37.23
• • •
50 -74
42.06
• • •
59.99
48.41
cc. Ethyl
Alcuholin
Mixtures.
3
6
9
12
IS
x8
flX
oc. HsO added to cause separation of a second phase
in miziures of the given amts. of Alcohol and 3 cc. of 1
CHvCICOOCiHa. CHQ]COOCta« CCliCOGCiH^
1.32
4.01
7.30
10. 78
x6.i6
22.16
28.74
0.90
2.45
0.65
X.80
4.33
6.60
9.20
3.02
4.50
6.50
• • •
• • •
• • .•
• • •
13
AOBTm
Mono-, Di-, and Tri ACETIN CaH,(OH),(OCH,0), C,H,(0H)(0C,H,0)2. and
C,H*(0C,H,O),.
Tae 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.
MethACSTlN {p Acetanisidine, or p oxymethylacetanilide) CeH4.0CHi.
NHCHjCO.
100 gms. HjO dissolve 0.19 gms. of the compound at 15° and 8.3 gms. at loo^
(German Phammoopoda.)
a ACBTNAPHTHAUDE CsHsONHCQoHt).
Solubility in Mixtures op Alcohol and Water at 25^
(HoOeman and Antusch — Rec. trav. chim. 13, 9891 1894.)
AIcoIkI
100
95
90
80
75
70
Gms. per
100 Gms.
Solvent.
4.02
4-31
4. II
318
2-73
2.31
Sp. Gr. of
Solutioos.
0.7916
0.8x50
0.8344
0.8485
0.8624
0.8761
0.8798
Alcohol.
65
60
55
50
35
20
10
Gms. per
100 Gms.
Solvent.
1.78
1.44
1.02
0.71
025
0.09
0.04
Sp. Gr. of
Solutions.
0.8977
0.9091
0-9201
0.9290
0-9537
0.9717
0.9841
Constant agitation was not employed. The mixtures were allowed to stand
in bath and the solutions analyz^ after different lengths of time. Formulas
are not given. This applies to all determinations by Holleman and Antush.
ACBTONS (CH,),CO.
Solubility of Acetone at 25® in Aqueous Solutions of:
Electrolytes. Non-Electrolyti
CBeU — J. Phys. Ch. Qb 544* 1905; Linebarger — Am. Ch. J. 24, 380, x8g2.)
Gms. ElectRH
Irtepec
no GtBB* A(|«
1.25
2.50
5 CO
7-5
10 .0
12.5
15 o
20.0
25 o
30. o
Gms. (CHa)aCO per 100 Gms.
Solvent in Somtions of:
/ * >
KiCOs NasCOs (NH4)2COs MgCOt
83 -5
no
73
65.0
46.5
34-5
255
18.0
8.0
3-7
X.6
51.0
38 o
275
195
14.0
9.0
2.7
57
44
35
28
o
5
o
5
o
o
65.0
47 o
38 o
29.0
Gms. Non-
Electrolyte
per 100 Gms.
Aq. Solution.
5
10
Gms. (CHs^sCO per zoo Gms.
Solvent m Solutions of:
. *
CioH^t Anethd.* (CeHft)sCO.
20
30
40
50
60
70
80
90
92
117
137
148
155
159
160
155
5
o
o
5
5
5
2
o
103.0
123.0
1445
15s o
162.0
166.0
165.0
158.0
90.0
108.5
126.0
133 o
136.0
135 -5
131-5
123 0
108.5
82.0
* Anethof - P Propenylanisol, CHs.CH:CH.C|H^CH«. f Naphthalene lesuhs 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, occurrra. 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.
AOBTONl
U
MlSOBILITY OF ACBTONB AT O^ WITH MIXTURES OP:
CMorafonn and Water (Bonner, 19x0).
Bzomobennne and Water (BoniM
/ *
Gms. Gms. Cms.
». x9»)-
Gma.
Gna.
Sp. Gr. of
Sp. Gr. of
CUO..
HdO. (CH«)sCX>.
Miztiue.
CABr.
w>.
(CHi).C0.
Mixture.
0.988
0.012 0.501
1. 18
0.977
0.023
0.685.
1. 12
0.900
O.IOO ]
C.3OO
1. 01
0.90
O.IO
113
1. 01
0.792
0.208 1
t-633
0.98
0.80
0.20
1. 41
0.98
0.696
0.304 ]
t.7So
0.96
0.70
0.30
152
0.97
0.600
0.400 ]
C.770
0.95
0.60
0.40
I 57
0.96
0.500
0.500 ]
[.720
0.94
0.50
0.50
1.60
0.9s
'0.420
0.580 ]
C.650
• ft •
♦0.49
0.51
1.60
• • •
0.400
0.600 ]
C.630
0.93
0.40
0.60
1-59
0.94
0.300
0.700 ]
C.S30
0.94
0.30
0.70
1. 55
0-93
0.200
0.800 ]
C.321
0.9s
0.20
0.80
1.46
0-93
O.IOO
0.900 ]
C.144
0.97
O.IO
0.90
1.30
0-93
0.018
0.982 C
>.464
0.98
. 0.02
0.98
0.849
0-9S
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 i>airs of liquids which may exist in eciuilibrium. When the two layers
are practicallv of tne 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.
(Knag and licEboy — J. Anal. Ch. 6^ 1841 '9»', Bdl — J. Phya. Ch. 9, 547f 'osO
Pcf cent
In Aqueous Solutions of Cane Sugar.
Cms. (CHa)iCO per 100 Gms. Sugar Soltttioo at:
10
20
30
35
40
45
50
55
60
65
70
if
597
272
172
5
4
• • •
• • •
96.4
71.9
50.8
35-8
25.2
18.3
13-9
581.8
250.0
150.0
• • •
92.8
68.8
48.1
33-8
24.2
17.7
12. 8
30"
574.8
251.8
150.6
4oS
« • •
• • •
• • •
• • •
1 10
85
62
42
29
In Aqueous Dextrose Solutions.
Gmi. (CHt)«CO per 100 Gma.
Solvent
Ptt
cent
Ivent at:
10
20
30
40
50
tf.
736.7
255-3
157-5
86.9
36.2
as".
747-9
247-7
149.8
79.6
33 o
35*.
761.5
240.8
142.5
74 o
31-3
Per
cent
Maltoae.
10
20
30
40
50
89.8
65 -7
45-9
325
23.4
17. o ••• •••
I2*s ••• •••
In Aqueous Maltose Solutions.
Gma. (CI
;Ha)iCO per 100 Gma.
Solvent at:
IS**.
353-6
185.4
119.9
78.4
46.2
as**.
348.1
181. 2
116. 0
74.7
42.9
35*.
342.0
176.9
112. 4
70.5
39-8
The determinations were made as in the case of the solubility of acetone in
aqueous solutions of electrol3rte8. See preceding page.
15
ACETONl
Distribution op Acbtonb bbtwbbn:
Benzene and
Results at 20^
Hp and Bnmby, 1915*)
Gm. (CHa>sCO per zooo oc
HdO
Layer.
O.IO
0.20
0.30
0.40
Layer.
0.08
0.12
0.25
0.34
Water.
Results at 25"*.
(Hers and Fischer, 1905.)
Cms. (CHt)tC0 per looo cc
Layer. Layer.
ID* 12.0
SO 41.7
100 IOI.5
ISO iSS-9
200 225.0
* See Note, page 6.
r.
o
10
20
30
Toluene and Water.
At Different Temps.
(Hant2sch and Vagi, 190X.)
Cms. (CH|)iC0 per looo cc
' hJo ' CjHiCHi
Layer. Layer.
2.105
2.000
1.960
1.867
0.993
0.957
0.957
0.957
Philip and Bramby also rive data for the effect of NaCl, KCl 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.
Distribution of Acbtonb bbtwbbn:
(Hers and Rathmann, 19x3.)
Water and
Water and
Water and
Carbon Tetrachloride.
Chloroform.
Pentachlorethane.
Mob. (CH|)sCO per Uter.
Mob. (CHOflCX) per Liter.
Mob. (CH,)tC0 per Liter.
W)
ca« :
W
CHCU
IW)
coicu
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
0.186
0.0833
0.032
0.168
0.144
0.251
0.322
0.146
0.0781
0.399
0.271
0.469
1. 01
0.514
0.145
0.676
0.541
0.859
1.66
0.997
0.263
1. 17
0.806
1.275
2.87
2.10
0.493
1.98
1. 149
1763
...
...
1. 01
306
• • .
...
Water and
Water and
Water and
Tetrachlorethane.
Tetrachlorethylene.
Trichlorethylene.
Mob. (CH,),0
0 per liter.
CACI4
Mob. (CHa)^CO per Liter.
' HjO CCJ,:CCi,
Mob. (CH,)tCO per Liter.
IV>
\H,0
CHChCdi
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
0.0812
0.341
0.274
0.081
0.160
0.193
0.249
0.994
0.562
0.174
0.350
0.359
0.317
1. 210
1.020
0.343
0.654
0.719
0.363
1.323
1.545
0.629
0.946
1.029
0.569 ^
1.936
2.007
0.891
1.389
1.562
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^
Sglubility Data Determinbd by thb Method of Lowering of thb
Freezing-point (see footnote, p. i) Are Given for Mixtures of Acetone
AND Each of the Following Compounds:
Bromine (Maanand Mcintosh, 19x2.) Phenol (Srhmidlin and Lang, xgxo.)
Chlorine " " Resorcinol
H vdrobromic Add " - Pyrogallol
Cnloroform (Takalotos and Goye, x9xo.) Pyrocatechol " "
o Chlorophenol (Bnunby, X916.)
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.
AGETOPHENOinB i6
ACETOPHENONE CH,COC«H«.
The freezing-poiiit curve for mixtures of acetophenone and sulfuric add is
given by Kendall and Carpenter (1914).
Freezing-point curves (solubility, see footnote, page i) for mixtures of Cinna-
mylidene Acttophonone and each of the following compounds are given by
Giua (19 16): Acenaphthene, azobenzene, ethyl ether and a trinitrotoluene.
AOBTTLAOETOHS CH,COCHaCOCH»
Solubility in 'Water.
CRodunund — Z. phys. Ch. 26^ 475, '98.)
Cms. CB,COUl,COCH,
per 100 Gms.
h9
HsO
Acetyl Acetone
9 •
Layer.
Layer.
30
15.46
95.02
40
17 58
93-68
50
20.23
91.90
60
23 23
89.41
70
27. ZO
85-77
80
33 93
78.8a
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, «.6., the solu-
bility of acetyl acetone in water; and the other represents the acetyl acetone
layer, «.6., 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, «.e., by analyzing each layer after complete separation occurs.
See also, chapter on Methods of Solubility Determinations.
ACETYLENE QH,.
Solubility in Water.
(Winkler; see Landolt and BOrsstein's Tabellen, 3d ed. p. 604, 'os.)
t*. «. q.
o 1.73 0.20
5 1.49 0.17
10 1. 31 0.15
IS I IS 0.13
20 1.03 0.12
2S 0.93 O.II
30 0.84 0.09
o, "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 grama
of the pure solvent at the given temperature if the total pressure, «.«., the partial
pressure of the gas plus the vapor pressure of the liquid at the absorption tem-
perature, b 760 mm.
17
ACSTTLENE
SOLUBIUTT OP ACBTYLBNB IN WaTBR, AqUEOUS SOLUTIONS OF ALKALIES AND
Sulfuric Acid at 15®.
(Billitaer, 190a.)
tn of Acetylene in Aq. Solutknifl of Nonnallty:
Aq.Sohitkn
•b U
1 nacvjuea
e in Aq.
oC:
o^x
0.035
. 0.0S
0.10
O.IS
Ba(OH)s
• « •
I.218
■ • •
1.230
1.240
Ca{OH),
1.230
• • •
• • •
NH4OH
1. 216
• • •
Z.218
NaOH
1. 210
1.200
I.180
KOH
I.2I2
• • •
1.185
Na,S04
• • •
• • •
1.170
H,S04
• « •
• • •
I.ZQO
0.25
aso
X.00
a.00
^•oo
1.220 1.225 1.230 1.235 1.240
1. 128 1.040 0.885 0.600 0.370
1. 130 1.056 0.912 0.660 0.460
1.068 0.940 0.720 0.340 . . .
1. 120 1.040 0.900 0.780
Solubility in Water, /u » 1.251.
.The above results were determined by the method of Ostwald (Handbuch
physiko-chemischen Messungen 207 if.). A thermostat was used and great
care taken to reduce experimental errors and purify the acetylene. The results
are in terms of the Ostwald SolubilUy Expression, for which see page 227, following.
SOLUBILITT OF ACETTLBNB IN AqUEOUS AcETONE SOLUTIONS.
(Kxemum and HSnel, 19x3.)
Vol. Per Cent H/>
in ^Tklv^fifr
Cms. CA dissolved per Liter Sat. Solution at:
lu sol vcm
(H/> + Acetone).
0*
i8*
-. _ ^
as*
0
37
21
iS-2
5
31
18.2
13. s
10
26
ISO
10. s
20
IS
9S
8.0
3S
8.4
S'S
. 4.4s
SO
5-7
1.23
2.22
75
...
...
1.23
100
...
• . .
0.98
Tlie freezing-point curve for mixture of acetylene and methyl ether are
given by Baume and German (191 1, 1914}.
Biiodide, da and trazis.
Data for the lowering of the freezing-points of mixtures of these two isomers
are given by Chavanne and Vos (1914J.
ACONinC ACID C,H,(CCX)H),.
too grams of formic acid (95% HCCK)H) dissolve 2.01 grams CsHt(COOH)i
at 20.6 C. (Aschan, 19x3.)
AOOHZTZVl (Amorphous) CmH4,NO„.
Solubility in Several Solvents.
(At 95* tJ3P.; at I8•-aa^ Mailer — Apoth.-Ztg. 18; a, '03.)
Gma. CnHcNOx per
xoo Gms. SolTent at:
Water .
Alcohol
Ether .
xS^-aa*.
0.054
...
X.44
0.031
4S4
2.27
Gma. GMH47NO11 pef
Solvent 100 Gms. SoiveDt at;
iV-aa*. 7f?
Benzene 17 -^S
Carbon Tetrachloride i .99
Petroleum Ether . . 0.023 0.028
100 gms. HtO dissolve 0.0226 gm. aconitine at 22^ (Dimstan and Umney, 189a.)
abs. alcohol " 2.7 " " " " auigens, 1885.)
" ether •*- 1.56 " ** " "
«<
M
<«
TVichloro4CBYLIG ACID
i8
TrichloroACBYLIC ACID CasK:aCOOH.
SCM^UBIUTT OF TUCHLOROACRYLIC AciD IN WATBR
(Boenkcn and Cazriere, igisO
O.O
—0.36
— o.6Eutec.
+13.7 "
150
17.0
19.2 m. pt.
ly.oEutec.
20.3
25.0
30.0
40.0
50.0
60.0
70.0
72.9
tt
cacooS
per 100 Gmk
Sat. Solution.
0.0
2.0
4.5
64.1
68.5
74.5
80.0
81. 1
82.8
84.5
86.0
89. s
92.5
94.5
98.S
100. o
Solid Phue.
ke
loe+COi: CaCOOH.a}H/>
ca»cacx)0H.2i h^o
CCl|:CaCOOH+
Cai:CaC00H.2}H/>
CCl|:CaCXX)H
(I
M
Between the concentration 4.5
and 64.1 two liquid layeiB are
formed. The percentage of
CClt:CCiCOOH in each is as
follows:
Gms. CCl|:CaCOOH per
t«. 100 Gms. Sat. Solution.
Lower Layer. Upper Layer^
SO
10
20
30
40
SO
S5
60
62 crit. t.
S.2
6.0
7.S
13 o
18.0
27.0
38.0
64.1
63.8
62.2
S9.S
S6.o
49.0
The original results were plot-
ted on cross-section paper and
the above figures read from the
curves.
ACTINIUM EBCANATIOKS.
SOLUBILITT IN SEVERAL SOLVENTS.
(Hevea/, 191 3-)
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 KCl, HA HjSOi, CxH*OH, CHuOH, (CHi),CO, C«H»CHO, OH*,
CtHs, petroleum ether and CS|. The solubility increases in the order named.
Close relations are indicated between actinium, thorium and radium.
ADIPIC ACID (Normal) (CHOiCCOOH),.
100 grams HsO dissolve 1.44 grams adipic acid at 15^
(Henzy — Compt. rend., 99f izS7i '84; Lamouiouz — Ihid., laS, 998, '99.)
ADIPINIC ACID (CH04(COOH)i.
ioo grams of formic acid (95% HCOOH) dissolve 4.04 grams of (CHs)4
(COOH}s at 18.5®; 100 cc. of the saturated solution contain 4.684 grams of
the acid. (Aschan, 1913.)
AGARIC ACID CioH»O..HiO.
100 grams trichloroethylene dissolve 0.014 gram agaric acid at 15^
(Water And Bnilnt« K914.)
19
Am
Solubility in Watbr.
CWiaUcr -» Bcr. 34. 1409, '01; ne also Pelcnan and Sondem — Bcr. aa» 1459* '89^
O
5
10
ao
25
30
40
SO
60
80
100
B '
B.
0.02881
.02543
.02264
.02045
.01869
.01724
.01606
.01418
.01297
.01216
.01126
.01105
0.02864
.02521
.02237
.02011
.01826
.01671
•01539
.01315
.01140
.00978
.00600
.00000
cc.* of atmoqphcric O and N per liter of:
DIat. HiO (at 760 mm.). Sea Water (at 760 mm.).
Oxygen.
10
8
7
7
6
5
5
4
3
3
I
o
.91
16.
.87
14.
.04
13-
•35
II.
•75
10.
•
.24
10.
.48
8.
•8S
?•
■ a8
6.
•97
4-
■00
0.
Nitrogen.
" 45
30
50
07
91
96
IS
67
55
50
03
00
OzTgen.
7-77
6 93
6.39
5 70
Nitrogen.
14.85
13-32
12.06
11.05
10.25
9.62
» '* Coefficient of Absorption," i,e,, the amount of gas dissolved
by the liqtiid when the presstire of the gas itself without the tension
of the liquid amounts to 760 mm.
J?' — •* 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* 389, '06.)
Wt. % H1SO4 98 90 80 70
SolubiUty Coef. 0.0173 o.(X369 0.0069 0.0055
60 50
0.0059 0.0076
Scx^ubility op Air in Alcohcx., btc
(Robinet, 1864.)
Sulvent.
Vols. Air per
Vols. Solvent.
xoo
Alcohol (95 . 1%) . . 14. 1
Petroleum 6.8
Benzene 14.0
SolTent.
Oil of Lavender. .
Oil of Turpentine .
Vols. Air per 100
Vob. Solvent.
• . 6.9
. . 24.2
(a Anunopropionic Acid) CH,CH(NH,)COOH.
Solubility in Mixtures op Alcohol and Water at 25®.
Vol.%
Alcohol.
O
5
zo
IS
90
«S
31
(HoOenMii and Antuch, 1894.)
Gms. per
100 Gms.
Solvent.
16.47
1437
"•43
10. 49
8.48
7. II
SS3
Sp. Gr. of
Sotutioos.
Vol.%
Alcohol.
Gms. per
xoo Gms.
Solvent.
I .0421 35 4
1.0311 40 3
1 .0280 50 2
1 .0101 60 I
o 9984 70 o
0.9886 80 o
o 9761
See remarks under a Acetnaphthalide, page 13.
100 gms. pyridine dissolve 0.16 gm. a alanine at 20-25^,
91
89
38
57
85
37
Sp. Gr. of
Soltttkos.
0.9670
0.9577
0.935s
0.9102
0.8836
o 8556
(Dehn, 1917.)
ALANINE
30
Solubility of d Alanine and of dl Alanine in Water at Different
Temperatures.
(Pdlini and Coppola, i9i3-)
Results for:
d Alanine.
d — l Alanine.
Mixtures i + / Alanine.
"' Gms. d Alanine per
Gms. d — l Alanine per
Gms. per
xoo Gms. I^.
zoo Gms. BbO.
xoo Gms. BbO.
J Alanine.
O 12-99
12.89
13-27
4.01
17 15.17
14.95
145
4.1
30 17.39
17.72
17 05
4.99
45 20.55'
21.58
• . •
• • •
ALBUMIN (Egg).
160 gms. HsO dissolve 100 gms. egg albumin at 20-25^ ku
100 gms. pyridine dissolve o.i gm. egg albumin at 20**-25°. *
100 gms. aq. 50% pyridine dissolve 6.29 gms. egg albumin at 20°-25**.
(Dehn, 19x7.)
(Dehn, Z917.)
ALLANTOm C4H6N4QS.
Solubility in Water.
(Titherly, 1912.)
The author obtained results varying from 0.7 to 0.77 gms. allantoin per 100
gms. HsO at 25^. The variations were considered to be due to alow decompo*
sition of the compound.
ALIZARIN Ci«HflO,(OH),.
Solubility in Water at Varying Temperatures.
(Hattig, X9X4; Beilstein.)
t". 25*^ «oo*. aso*.
Grams Alizarin per liter o .000595 o .340 3 .017
According to Dehn (1917), 100 gms. HsO dissolve 0.04 gm. alizarin at 20^-25^
Solubility of Alizarin in Aqueous Solutions of:
Sodium Hydroxide at 25° (Httttig, 1914.)
Ammonia at 25**.
-*-
Gms. NHiper
Liter.
0.160
4.025
Gms. Alizarin
p>er Liter.
0.132
0.228
Gms. NaOH
per Liter.
0.427
1.050
Gms. Alizarin
per Liter.
1. 159
3.820
SoUd Phase.
C14HA
C14H8O4 + Ci4H704Na
too gms. 95% formic acid dissolve o.io gm. alizarin at 20.8^. (Aschan, X9X3.)
Alizarin is soluble in all proportions in pyridine and in aq. 50% pyridine at
2o'*-25'
(Dehn, 19x7.)
ALOm.
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^
31
ALUMDHUM BBOBODE
ALUMINIUH BBOMIDX AlBri.
SOLUBTLTTY IN SEVERAL ORGANIC SOLVENTS.
(Menachutkin, 1909-10.)
(Determiiiatioiis by Synthetic Method.)
In Benzene.
In Para Xylene.
• GiiLs. AlBn per
Gma. AIBn
per
i
li*. xoo Gms. Sat.
Solid Phue.
r
\ xoo Gms. Sat. SoUd Phaie.
SoL
SoL
S-ym. pt 0
CA
14 m
. pt.
0
^C.B«(CH^«
4S
ID
M
12. s
II.4
f
3
20
M
10.2
Eutec.
2S
AlBn+# QH<(CHi)t
i.SEutec. 27.4
(CA+AIBi^
20
3S-7
AlBi^
10
35-3
AIBn
30
47.2
M
20
46.5
M
40
61.2
M
30
S9
M
so
72.2
«
40
70
U
60
79.6
«
60
83
U
80
90.9
M
80
91.2
U
90
95. 4
«
90
95-3
U
96
100
«
96
100
M
In Toluene.
In Benzoyl Chloride.
J*
Gms. AlBa
^ r
Gms. AIBn
f.
per 100 Gna. SoKd Phue. t*.
per xoo Gnu
>.
Solid Phase.
Sit. SoL
Sat. SoL
-IS
16. 1 AIBn
- o-S
m. pt.
0
Ci&coa
0
23.7
- 2.5
II. 7
«
10
32.1
- S
Eutec.
22.2
C|HiOOa+AlBn.C|HiCOa
20
42s
20
33-7
AlBn.C|&COa
30
56
40
42.6
M
40
68.8
60
51.6
M
5°
76. s
80
60.5
M
70
87.2
90
m. pt.
^S'S
M
90
95-7
80
68.9
«
96
100 "
60
30
71.8
7S-8
«
M
7
Eutec.
78.8
AIBn-CHiCOa+AIBri
30
80.6
AIBn
SO
85.6
M
80
93-2
M
96
100
a
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 AlumlTiliim Bromida 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 Bromida and dimethylpyrone are given by Plot-
nikow (1911)-
ALUMINZUM BBOMIDE
SoLUBiLiry OP Aluminium Bromidb in Sbvbeal Organic Solvents (Con.')
(Determinatioiis by Synthetic Method.)
In Benzopli
lenone.
In Ethylene BromideJ
Cms. AlBnpa
K
Gms. AlBife
... _ , ,
per
t*. zoo Gm. Sat.
Solid Phue.
f. zooGm.Sat. SolidPhaaeJ 1
■
SoL
Sol.
,
48 m. pt
0
(cja^^co
10 m. pt. 0
CABife
4S
12
*•
6 II. s
It
42
19
M
2 21.3
ff
38 Eutec.
24.7
** +AlBn.(C>Hi)«C0
— 2 Eutec. 29.7
CABti+AlBn
60
30.9
AlBn.(CiHi)tC0
10 36.1
AlRn
80
36.4
w
20 42 . I
<f
100
42.2
M
30 48.7
«
120
49
M
40 S6
a
130
S3
M
SO 63.7
«
142 m. pt.
S9-5
M
60 71.5
M
130
64
M
70 79.1
M
100
69
«
80 86.8
M
70
72.2
M
90 94. S
m
SO
74
«
96 100
m
38 Eutec.
7S
** +AIBII
50
78
AlBo
80
88
. M
90
93S
m
96
100
m
In Nitrobenzene.
In 0 Chloronitrobenzene.
Gms. AlBn pa
«
Gms. AIBciper
. . . . ^
t*. zoo Gm. Sat.
Solid Phase.
t". zoo Gm. Sat.
SoUd Phase.
Sol.
Sol.
S.Sm.pt.
0 QHiNOi
32-
5 m. pt. 0 0 CiHiClNQi
0
18
If
25
21.8 "
-s
28.8
M
13-
8 Eutec. 37.5 " +AlBi»u» C,HiClN0i
-IS Eutec.
42
" +AlBn.C|Ha^0i
30
43 . 1 MBn^ C|H«ClN0i
0
44-3
AIBQ.C«IbN0i
SO
so. 3
t0
30
49-4
u
70
57.6
«
60
S6.7
M
83-
5m.pt. 62.9
tt
80
63.6
U
70
67
M
87 m. pt.
68.4
«
40
73-7
«
•
80
71.3
«
21
Eutec. 77.5
" +AlBia
60
73-9
M
40
80.6
AlBn
40
;6.4
M
60
84
«
20 Eutec.
78.9
'* +AlBn
80
8S.6
u
40
82.4
AIBn
90
93-4
u-
60
85.8
u
96
100
M
80
89.8
M
93
96.6
M
96
100
M
23 ALUMDHUM BBOMIDE
SOLUBILITT OF AlUIONIUM BrOMIDB IN SEVERAL ORGANIC SOLVENTS (Con.).
(Determinations by Synthetic Method.)
In m Chloronitrobenzene.
Cms. AlBnper
t*. iooGms.Sat. Solid Phase.
SoL
44.5m.pt. O wCtHtONOi
40 18.9 "
35.5 EuteC. 27 . 8 "+AlBiw» CJEUONCh
50 34.8 AIBn.111 Ci&CINOi
70 44. S
90 545
103.5 m. pt. 62.9
90 68.6
70 73-4
SO 77.3
40 EuteC 79 . 1 " +AlBri
60 82.2 AIBq
80 87.1
90 92.2 "
95 9SI
96 100 *
H
<f
If
M
In p Chloronitrobenzene.
Gma. AIBq per
t*^ 100 Gma. Sat. Solid Phase.
•SoL
83 m. pt. O P C^ONOi
80 9 "
70 24.8 "
60 EuteC. 36.6 " +AlBn.^ caciNOi
80 45 . 6 AlBn.^ CAClNOi
100 54.9
115 m. pt. 62.9 ••
100 66.8
60 72.4 "*
20 Eutec. 78 - +AiBft
60 85.3 AlBn
80 89.3
93 95-4
96 100 *
In o Bromonitrobenzene.
(
Bm. AlBn l
per
r.
loo GnH. Sat. SoUd Pfaiae.
SoL
38 m. pt.
0 a
.CiHiBtNOi
30
19.7
U
21 Eutec.
30
" +AlBnj> C«H4BrN0i
40
37-6
A1Be»» CgHiBrNOi
60
45-3
<€
80
53
II
88.5 m. pt. 56.9
II
80
59-7
14
60
64.1
M
40
68.6
W
24 Eutec.
72
"+AlBtt
40
7SS
AlBn
60
79.8
If
80
86.3
(f
93
945
«f
96
100
a
In m Bromonitrobenzene.
, _-« ,
Gms. AlBn per
t*. xoo Gms. Sat. Solid Phase.
SoL
54 m. pt. O MQHiBrNOh
50 II. 6 "
45 . 5 Eutec. 19 . 5 "+AlBft.» CaBrNOi
60 25.5 AlBrs.« CiHiBrNOi
80 34.5
iio 49.5
I22m.pt. 56.9 "
IIO 61.6 **
80 69.2 "
60 74.1 *•
42 Eutec. 78 . 7 " +AIBn
60 80.3 AlBn
80 84.9
93 93-6
96 100
M
ff
ALUmNIXIM BBOMIDE 24
SCX^UBILITY OP AlUMINIITM BrOMIDB IN SEVERAL ORGANIC SOLVENTS (Can.).
(Determinations by Synthetic Method.)
In p Bromonitrobenzene.
In p Nitrotoluene.
Gnu. AlBr< L
Der
(
Qms. AIBn
Der
■%
t°. 100 Cms. Silt. Solid Phase.
f.
xooGins. Sat.
Solid Phase.
Sol.
Sd.
124.5 ni.pt
. 0 >.C«EtBrNOi
S3.sm.pt. 0 pcjEucHtsot
119
10
«
so
10
((
no
25.2
IC
40
313
u
98 Eutec.
55-3
"+AlBn.^C«H4BrN0i
29 Eutec.
46.1
"+AlBi».^CJH4CffiN0»
no
39-7
AlBife.^ CiHiBrNOi
SO
52.9
AlBQ.^C»HiCH«NOh
130
48.7
M
80
63
M
144 m. pt.
56.9
«
88 m. pt.
66
«
120
65.5
u
80
68. s
M
90
70. S
M
5°
74.3
U
60
74.1
a
27 Eutec
78.9
" +AlBn
45 Eutec
76
"+AlBn
SO
83.3
AIBn
60
79.6
AIBn
70
87.7
M
80
86.6
M
8S
92.2
M
93
95-4
a
93
96.7
M
96
100
«
96
100
«
In m Nitrotoluene.
Gms. AIBn
t*. per zoo Gms.
Sat. SoL
Solid Phase.
16 m. pt. o
12 14. s
8 21.8
I Eutec. 32
20 38. s
40 46.6
80 S9-7
90 63.3
96 m. pt. ^6
90 68.8
60 73.8
27 Eutec. 78.9
40 82
70 89
90 95 -3
96 100
CcHiCHiNOi
ft
M
■> r
In 0 Nitrotoluene.
f.
Gms. AlBrs
per xoo Gms.
Sat. Sol.
SoUd Phase.
"+AIBQ.111 CHiCHiNOi
AlBn.« CACHiNOi
— 8.S m. pt.
— II Eutec.
10
30
40
u
" +A1BQ
AIBn
M
tt
42. s Eutea 47.7
O « C«HiCHiNOi
8 . 7 <*+AIBn.2aC»HiCH«N0i
12.8 AIBn.3aC«HcCHiN0i
24.8 "
38.
60
7S
90 m. pt.
70
40
19 Eutec.
40
70
90
96
543
595
66
72
76.1
79.1
82. s
87. S
93.8
100
'+AIBnMC«HiCH^Oi
AlBnuv CHiCHsNOh
M
"+AIBQ
AIBn
u
25
ALUMINIUM CHLORIDE
ALUMDHUM CHLOBIDE A1C1<.6H,0.
Solubility in Water.
(Gerlach — Z. anal. Ch. 8, 350, '69.)
100 gms. saturated solution contain 41.13 gms. AlCU at i5^Sp. Gr. of solu-
tion » 1.354-
SOLUBfLITT OF AlUMINIITM ChLORIDB IN SEVERAL ORGANIC SOLVENTS.
(Maiachutkln, 1909.)
(Determinations by Synthetic Method.)
In Nitrobenzene.
In 0
Chloronitrobenzene.
a
Gn». AlCb
Gms. AlCb
%
t*. per xoo Gms.
Solid Phase.
r.
per xoo Gms.
Solid Phase.
Sat.SoL
SaLSoL
5.Sm. pt. 0 C«HiNOi
32 . 5 m. pt. 0 » c^ONOi
2Eutec. 10.3 •
• +Aiaa.2CHiN0i
27
10.2 "
15 18 AlOs-aC^HsNOi
21
16. 1 "
25.5 Eutec 30.5 '
• +Aiai.C,H,N0,
15 Eutec
20.3 "
+AlCb.0C«H4ClNOi
45 34.2
AlCb-CHiNOi
35
25.5 AlCb.a CeHcONOi
65 395
(f
SS
3IS
u
85 48
If
75
38.7
u
90 m. pt. 52
it
89 m. pt.
459
u
82 55. 6
M
80
SI
u
72 58
M
69 Eutec.
544
"+AlCb
52£utec 61.6
"+A1C1,
no
S7S
AlCb
90 64
AlCb
ISO
65.4
<i
130 67 . 7
a
175
74.6
M
160 72.4
w
194
100
M
180 80.1
u
194 100
M
Iniff Chloronitrobenzene.
•
In p Chloronitrobenzene.
Gms. AlCb
\
Gms. AlCb
■ -■ >
t*. per xoo Qua.
SoFid Phase.
f.
per xoo GiQs.
Solid Phase.
Sat,SoL
Sat. Sol. .
44.5111. pt.O mCcHcCINOi
83 .5 m. pt. 0 ^CeHiONOi
44 10.7 «
78
7.1 "
36£utec. 16.6 "+Aici..iiiC»ciNOi
73
li2.8 "
50 21 AlCb jn CiHidNOi
68 Eutec.
17. 1 "
+AlCb.^CJH4ClN0i
70 28.3
u
80
22.2 AlCb.^C4H<aN0i
90 36.8
M
100
314
M
IQ4m.pt 45.9
M
120
41.8
«
90 52.4
fl
126 m. pt.
45-9
(€
81 Eutec. 55.6
"+AlCb
no
53-2
U
120 60
AlCb
94 Eutec
58.1
"+AlCb
140 64.1
.11
125
60.5
AlCb
160 70.2
«
^SS
66.9
(f
180
77.7
«
190
88.2
M
194
100
<l
The solubility of aluminium chloride in anhydrous hydrazine is stated by
Weldi and Broderson (19 15) to be i.o gm. in 100 cc. at room temperature.
ALUMINIUM CBLOBIDI
26
Solubility in Several Organic S(x.vbnts (Can.),
(Determinatioiis by Synthetic Method.)
In 0 Bromonitrobenzene.
In m Bromonitrobenzene.
Gnu. AlCk
Gma-AlOs
»
f . per ue Cm. Solid Phi«.
t*. per xoo Gms.
Solid Phue.
S«t.SoL
SatSoL
38.S
0 0
CHiBrNOi
54.7 0 -
CHarNOi
32
7-S
If
SI 6.S
u
a6
13 I
M
47 Eutec. II. 9
"+AlCbjiiCiHiBrNOi
2o£utec
I7S
''+AlCb^CiH4BrN0i
60 16
AlCb4»QHiBrN0ft
40
21.7
AlCW CiHiBrNOft
80 22.9
«f
60
26.4
€«
100 30.7
M
80
31-7
M
"o 35-9
M •
97 m. pt
38
fl
116 m. pt. 39.8
U
100
39-8
M
113 42.3
M
90
44.6
U
107 44. S
m
SoEutec.
46. s
" +Aiai
97 Eutec 47.4
«+AlCb
no
SOI
Aid,
120 51.5
AlCb
130
541
a
140 56.5
M
150
60. a
M
160 64.5
«
170
70
M
180 77.4
<t
180
77-4
«
190 88.8
197 100
«
•
In p Bromonitrobenzene.
In 0 Nitrotoluene.
Gnu. Aids
f*. per xoo Gms.
SaLSoL
Solid Phue.
124.5 m. pt.O #CiHiBrNQi
117 7.4 "
III 12.8 "
loS 177 "
99 Eutec. 22 . 2
120 28.4
140 36 .4
14Sm.pt. 39.8
140 44.5
120 51.2
113 Eutec. 52.8
130 SS-9
150 61 .3
180 77.4
190 88.8
Gms. AlCb
t^. per xoo Gms.
Set.SoL
Solid Phase.
— 8.5 m. pt. O «C«HiCHsNOfe
— 9.3 Eutec I "+AlCU.acC,HiCHiNO*
O I.5AlCb.atfC»HiCHsN0i
20 4 "
"+Aia..# Cill«BrNOi
40 II
M
AlOs-^C^HiBrNOft
SS Eutec 31
" +AlCUu» QHiCHiNO*
M
Ss 41.8
AlCW CcHiCHsNOft
M
95.Sm. pt.49.3
M
U
1
70 S6.8
M
<(
45 Eutec. 61. s
••+Aiat
•*+Aiat
9S 64.5
AlCb
AlOi
I4S 73-7
M
u
180 86.2
M
M
185 89. s
M
«f
194 100
«
u
194 100. o
One liter sat. solution of Aid in CCI4 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 AlGa in CHGs contains 0.65 gm. at —15^1 i.o gm at
o"* and 0.72 gm. at 25^
(Lloyd, X9x80
27
ALUMINZUM C#HLOBIDE
SOLtTBILITT IN SEVERAL ORGANIC SOLVENTS (CoH.).
(Determinations by Synthetic Method.)
In m Nitrotoluene.
In ^ Nitrotoluene.
GmB. AlCh
Gms. AlCls
t*. per loo Gma
. Solid Phase.
t^. perzoo Gms.
Solid Phase.
SatSoL
Sat. Sol.
i6 m. pt«
0 m
CiHiCHtNOi
53.5m.pt. 0 ^(VEtCHiNOk
13 Eutec
7.8 -
+AICI1.3111 CiHiCHiNOi
47
9.2 "
27
13 .4 Aiaa.2m c^casot
42
15 "
35 Eutec.
24. 5 "
' +A]Cb.iiiC»HiCEbNOi
37
Eutec. 19 "+A1CU.^CACH,N0,
6S
34
AIOmkCHiCHiNOi
55
29.1 AlCli.^ C«HiCH,NOi
90
44.2
a
80
34.8
M
95
46.7
u
95
41.3
M
Q9.Sm.pt. 49.3
M
109
m. pt. 49.3
«
70
56.8
t€
100
53.4
«
45 Eutec
61. s
"+Aiat
60
61.7
M
9S
64. S
AlCb
45
Eutec. 64
^+Aiai
120
68.2
M
los
69.5
AlCb
130
70.2
«
165
80
M
190
94.3
M
194
100. 0
«
In Benzophenone.
In Benzoyl Chloride.
Gnu. AlCls
Gms. AlCb
^
r.
per xoo Gma. Solid Phaie.
t*. per 100 Gms. Solid Phase.
Sat. SoL
Sat.Sol.
•
48 m. pt.
0 {
:cw)«co
— 0.
; m. pt. 0 CiHiCoa
44
8.5
ft
-4
7.9
M
39.5 Eutec- 15.4
" +Aiai(CH«)«co
—7.5 Eutec. 12.7
" +Aicu.cH.coa
60
19.3
AlClt.(C«Hi)tCO
0
14. 1
Aiai.CiHiCoa
90
26. s
M
20
18.8
M
120
37
a
40
25
M
130 m. pt.
42.3
u
60
33
«
no
48.8
M
80
42.2
«
80
53-5
M
93m.pt. 48.7
M
60 Eutec.
56.1
**+Aiai
80
52.9
a
100
58
AlCb
60
57.2
«
140
63
u
40
61
m
160
68.6
«
180
78:5
«
190
89.1
M
192
93
u
194
100
«
ALmmVIUM FLUOBTOE AlF..
Fusion-point data (Solubility, see footnote, page l) are given by Pushin and
Baskov (1913) for the following mixtures:
AlF, + NaF, AlF, + KF, AlF, + LiF, AlF, + CsF, AlF, + RbF.
Similar data for mixtures of AlF, + NaF are given by Fedotieff and lUjinsky
(1913).
ALUMIIIIUM HYDROXIDE
28
4L17MI1IIUM HTDBOXIDE Al(OH)t.
SCX^UBILITY OF MoiST FrSSHLY PREaPITATBD ALUMINnTM HTDROXIDB IN
Aqueous S(H«utions of Aluminium Sulphate.
(Krenunn and HQttinger, 1908.)
Results at 20'
Results at 40^
Cms. per 100 Gms. H«0.
Solid Phase.
u
AkCSOO*. Al(0H)i.
2 .37 0.15 AIsOs-SOs-qHsO
S 030
7 0.6s
9.1 1 .30 Transition Point
10 1.23 AIA2SQ8.12H9O
IS I 04
20 I .40
25 2.40
30 3.70
31.6 4 . 20 Transition Point
33 2.7s Al«Oi.3SQ».i6HaO
34.73 0.92 "
Gma. per icx> Gms. HgQ.
A1,(S04)^
5.22
Solid Phase.
(I
tt
tt
It
Al(0H)s.
1.33 Al2O8.SOa.9H2O
. . .* Transition Point
8.85 1.82 Al202.2S08l2H«0
10 1.65
IS I .40
20 2.15
25 3 80
28 . s 5 . 80 Transition Point
30 4. 35 Al,Os.3SO«.i6H20
35 1.60
49 0.60 ''
Results at 60".!
U
Gms. per 100 Gms. I^.
Solid Phase.
* The figuies given are not niffident to deters
mine this transition point accurately.
t The author's figures for 60* are reproduced
without change as th^ are not sufficient to deter-
mine transition points.
it
AliCSOO*. Al(0H)i.
3 . 24 0.75 AlsOs.SOs.9H2O
8.83 2.53 AISO3.2SO8.I2H2O
12.67 1.85
24.07 3.14
31.55 4.89
42.38 6.02 Al20a.3S08.i6H20
.49.85 1.42 "
Solubility of Aluminium Hydroxidb in Aqueous Sodium Hydroxide
Solutions. (Haber and van Oordt, r904.)
The mixtures were agitated for 24 hours. So-called acetic acid soluble Umerde
(E. Merdc) was used for the experiments. Temp. 20^-23^.
Normality of Aq. NaOH. Gms. AkOi per Liter.
0.49 9.27
0.99 13.90
2.00 14.40
Solubility op Aluminium Hydroxide in Aqueous Solutions of Sodium
Hydroxide. (Herz, 1911; Slade, 191Z and I9XS-)
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 : i in normal NaOH at 25^ for cold pre-
cipitated hydroxide dned over HtSOi and 9.0 : i for hot precipitated Al hydroxide
dried over PsOs. Drying in thin layers also increased this ratio but to a some-
what less extent. Slade reports the solubility of Al(OH)t in a 0.6414 normal
NaOH solution to be 1.34 gm. per 100 cc. at room temperature.
ALUmNIXIM OXmE AltOt.
Fusion-point lowering data for mixtures of aluminium oxide and cryolite are
given by Lorenz, Jabs and Eitel (1913). The results show one eutectic at ap-
proximately 940^. The eutectic mixture contains 19.8% AlsOs.
Results for aluminium oxide and magnesium oxide are given by Rankin and
Merwin (1916).
29 ALUMimUM SULFATE
ALUMINIUM SULFATE Als(SO«)t.i8HtO.
Solubility in Water.
(Posgiok, XS43; Kremum aad HQttinger, 1908.)
*•• f^cSi^'Sf SoMPhu.. V. '^clJlf^'irLSoUdPbue.
- 1.02 8.09 Ice 20 26.7 Ali<SO0a.x8aO
- 1.43 10.7 " 30 28.8
-2.04 14 -3 " 40 31 -4
- 2.6s 17 S " so 34-3
— 2.85 19.2 " 60 37.2
- 4 EuteC. 23.1 Ice + Al«(SO.)«.x8HiO 70 39.8
o . 23.8 Aii(soo«.x8ao 80 42.2
+ 7-73 24.8 " 90 44.7
10 25.1 " 100 47.1 "
SCH^UBILITY OF AlUMINIITM SULFATB IN AQUBOUS SOLUTIONS OF FBRRIC
Sulfate at 25^ and Vice Versa. (Wiith and Bakke, 19x4)
Cms. per 100 Gms. Sat. Sol. «,.«*.. • Gvaa,. per xoo Cms. Sat. Sol. ^ ,. , _
, * » Solid Phase. < . * ■» Solid Phase.
AlKSOOa. • Fei(SO0«. AU(SOi)i. Fe«(SO0».
27.82 O A]i<SO0a.i8HsO IO.O3 32.42 FeiCSOJi-gH^O
26.01 6.064 " 8.819 34<^2
24.21 9.819 " 6.626 3582
21.64 13 02 " 5.200 38.83
15.22 23.28 *' 2.342 42.44
10.46 31-90 " +FeKS0«)i.9Hi0 ... 44-97
€1
<l
(I
Equiubrium between Aluminium Sulfate, Lithium Sulfate, and Water
AT 30^. (Schreineiiiaker and De Waal, X906.)
Gmpositian in Weight pa cent:
/— — ■* \ Solid
Of Solution. Of Residue. ^^
%Li,S04. %Al,(S04)i. %Ii«SO«. %Al,(S04)t.
25 . 1 O • . . ' - . U^4.H^
u
It
21-93 S-34
16.10 14.89 63.70 4. 02
13.63 20.76 14.72 3II7 {^^^-g^.I^H^
13.24 21.71 61.24 7.22 U^SO».4HtO
11.73 22.08 6.92 33 54 Al,(S04)i.x8HjO
6.7s 24.34 3.77 37.06
3 .44 26.12 • • • • . • '*
Q.O 28 .0 - • • • • • "
Solubility of Aluminium Sulfate in Aqueous Solutions of Sulfuric
Acm AT 25*. (Wirth, xgxa.)
Gma. per xoo Gms. Sat. Sol. ^ ,..«,. Oma. per xoo Cms. Sat Sol. „ ...*..
4 '^ * > Solid Phase. < * > Solid Phase.'
rSCsOoI HiSOi. ^'^w^™*- AWSOOt. HiSOi. ooua rMsc.
27.82 O A]|(SOi)s.x8HiO 4.8 40 A]|<SO0a.x8IbO
29.21 5.13 " 1.5 50
26.2 10 " I 60 "
19.5 20 " 2.3 70
II. 6 30 " 4 75
A curve was plotted from the published results and the above figures read
from the curve.
100 gms. glycol dissolve 16.82 gms. AltCSO^i. (de Coninck, 1905.)
ALUMINIUM SULFIDE A1,S|.
Fusion-point data for mixtures of AltSi + AgsS are given by Gimbi (1912).
ALU1I8
ALUMS.
do
SoLUBiLiTT OP Ammonium Alum and op Potassium Alum
IN Water.
(Mnkkr; Poggiale — Ann. diim. phys. [3] St 467. '43I Locke — Am.Ch. J.a6, 174. 'oi; Madno—
GasB. chim. ital. 35, II. 35X1 '05; Berkeley — Thus. Roy. Soc. 303 A. 9x4, '04.)
O
S
zo
15
20
2S
30
40
SO
60
70
80
90
92 S
9S
Ammoninm Alum.
Gms.
Al.(l
(NHJs Gms. (NH|)s G.M.Qmi)s
:SO«)« Als(SO«)«a4H>0 A1s(SQ«)a
per xoog.
3.10
3
4
6
7
9
10
14
ao
a6
SO
99
2S
74
19
94
88
10
70
109
per 100 g.
HsO.
3
6
9
12
IS
19
32
30
44
66
90
91
S2
66
13
19
01
92
10
65
per xoog.
HaO.
0.0044
OK>074
0.0105
0.0132
0.0163
0.0194
0.0231
0.0314
0.0424
0.0569
Potasaittm Alum.
■ A
Gms.Ka
A]«(Sq3«
per xoo g.
HaO.
30
35
4.0
S-o
5-9
7 23
8.39
11.70
17.00
24 -75
40.0
71.0
109.0
119. o
Gms. Kf G. M. K|
M^S0^4»aB^ AIsCSOJa
per xoo g. per xoo g.
HsO. « H«0.
0.0058
0.0068
0.0077
0.0097
O.OII4
0.0140
0.0162
0.0227
0.0329
0.0479
0.0774
0.1374
0.2II0
0.2313
5-65
6.62
7.60
9S9
11.40
14.14-
16.58
23 83
36 40
S7-3S
110.5
321.3
2275.0
00*
00
0.3313
Note. — The potassitun alum figures in the preceding table were
taken from a curve plotted from the closely agreeing determinations of
Mttlder, 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 ammonitim and potassitun altun 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 altim figures given above were
therefore read from Poggiale's potassium alum curve, with which
Locke's determination of the solubility of ammonium alum at 35^ is in
entire harmony.
Solubility op Ammonium Alum in Presence op Abimonium Sulpate and m
Pkesbncb op Aluminium Sulpate in Watbr^
CRfldorff — Ber. i8» izte, '85.)
Mixture Used.
zoo Gms. Saturated Solutioii Contain:
Saturated Ammonium Alum at 18.5^ . . . .
30 CO. above sol. -h 6 gms. cryst. Ala(S04), .
3o cc. above sol. + 4 gms. cryst. (NH«)2S04.
Gnias (NH0^SO4 + Grams Ala(SOi)».
. . 1.43 3.69
0.4s
30.81
16.09
0.39
31
ALUMS
Solubility of Mixtures op Potassium Alum and Aluminium Sulfate
AND OF Potassium Alum and Potassium Sulfate in Water.
(Marino — Gam. cfaim. itaL 35. H. 351. '05.)
*•.
Cms. per looe
Oms. HsO.
Gm. Mob. per 1000 Mob. Eb
V
Ala(Sa0s.i8HaO.
KaSd«.
A]a(S04)s.i8HsO
. KtSO«.
0
243-73
23-45
6.1
^'3
30
824.25
30.85
iS-i
3-1
35
911.02
35-29
24.1
3-6
SO
1243-21
S9-SS
33 S
6.1
65
159^ 00
"9-43
43-1
12.6
77
1872 . II
183.80
So-5
18.9
0
5.06
75-83
0.1 •
7.8
o-S
8.66
75-18
0.2
7-7
S-
16.07
85.78
0.4
8.8
10
18.52
96.50
0.5
9-9
IS
20. 56
109.30
0-55
II. 2
30
39 60
147.8
I.O
15-2
40
73.88
163. 1
1.9
16.8
so
126.0
195-4
3-4
20.1
60
249-7
238.8
6.7
24.6
70
529. 0
323-7
14.2
32.6
3o
1044 0
517-27
28.1
S3 -4
Solid
Phase.
K^(S0,),.a4H,O
+ AI,(SO0.
it
ii
ii
€i
K^(SO0,.34H,O
it
it
U
u
ii
ti
it
u
u
Solubility of Mixtures of Potassium Alum and of Thallium
Alum in Water at 25**.
(Fock — Z. Kryst. Min. aS, 397, '97.)
K^(S0J,.24H,0; T1^(S0J,.24H,0.
ComporidaQ of Solution.
KAKS0«)9 per Liter.
Grams.
69.90
74 56
67.90
65 30
64 95
53-23
45 32
38.0a
34-54
28.3s
10.94
o
Big. Mols.
270.5
288.2
262.8
252.7
251-4
205.9
175-4
147-2
^33^
109.7
42.4
0-0
'nAl(S04>i per Uter.
Grains. Mg. Mols'.
0.00
0.48
1.72
452
9.60
18.44
24.60
32.48
35-59
42.99
66.12
75 46
0.00
1-13
4.07
10.67
22.67
43 56
58.10
76.75
84.10
101.60
156.2
178.3
Mol.%
KAl(S04)a.
100
99.61
98.48
95-95
91-73
82.54
75-"
65-73
61.36
51-93
21.34
0.00
Sp. Gr. of
SolutioDs.
0591
0601
0598
0603
0605
0609
0609
0611
0611
0623
0654
0674
Sdid Phase
Mol.% of
PoCaaaium
Alum.
100. 0
9932
96.84
90.84
82.94
68.24
58.23
46.72
4423
32 07
7-94
0.00
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 Aliuns are given on p. 582.
ALU1I8
32
SoLUBiLiTT OP Sodium Alum in Water.
(Smith, 1909.)
Cms. NaaAli(S04)« per xoo Cms.
* .
Sat. Sol.
Water.
10
26.9
36.7
15
27.9
38.7
20
29
40.9
25
301
431
30
31 -4
45-8
f.
Gms.NaiAl>(SO0
1.34H1O per 100 Cms
Sat. Sol.
Water.
10
S0.8
103. 1
IS
52-7
III. 3
20
54-8
121 .4
25
56 -9
131. 8
30
59-4
146.3
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 op Caesium Alum, Rubidium Alum, and op Thallium
Alum in Water.
Roy.
Soc. ao3 A, 915, '04.)
'» •w^I 'V
Caesium Alum.
Rubidium Alum.
Thallium Alum.
t*
Gms. per 100
Gms. H2O.
Gms. per 100 Gms. H2O.
Gms. per 100
Gms. H3O.
• .
AlsCsa(S04)4.
Al2Cs2(SO;)4
.34HsO.
AlaRbs(S04)4.
Al,Rbs(SO;)«
.34HsO.
AlsTlaCSGJ^.
AlaTI,<S04)*
.34H20.
0
0.21
0.34
0.72
1. 21
315
4.84
s
0.25
0.40
0.86
1.48
3-
80
5-86
10
0.30
0.49
1.05
1. 81
4-
60
7.12
20
0.40
0.65
1.50
2-59
6.
40
10.00
25
0.50
0.81
1.80
3"
7-
60
"•95
30
0.60
0.97
2.20
3 82
9-
38
14.89
40
0.85
1.38
3-25
5-69
14.
40
23 -57
50
1.30
2. II
4.80
8.50
22.
so
38 41
60
2.00
3 27
7.40
13 36
35-
36
65.19
70
3.20
527
12.40
23 25
• I
•
• • •
80
5 40
9 01
21.60
43 25
• fl
«
• • •
90
10.50
18. II
...
• . •
• ■
■
• • •
100
Tk.T
22.70
/-*
42.54
4 M
• . *
J •• # A
...
« * <
■ 1
1 •
4
• « •
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 sdums see page 180.
SoLUBiLrTY OF Ammonium Chromium Altmi in Water.
(Koppel, 1906.)
It was shown that, due to the transition between the violet and ^preen 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.
o
30
40
Time of Gms.
Saturation, (NH«) Cr (S0«)s
Hra. Iter zoo Gms. Sol.
2-5 3-8
2.5 10.6
2-5 ^5S
f.
Time of
Saturation,
Hra.
0
2.5
30
300
40
250
Gms.
(NH^)Cr(S0dt
pa zoo Gms. SoL
3-8
15-7-16
24.5-24.8
53
AMMONIA
AMMOHIA NH,.
Solubility op Ammonia in Water.
— Liebig's AniuJen, xia, 334, '59; Raoolt — Ann. chim. [5] x, s6a, '74;
Am. Ch. J. xgb 807, '97^
At j6o nm.
Pressure*
t\
per xoog.
• Pressure*
♦•.
C. NH«
per xoog.
HsO.
Vol.Nfit
per X g.
Vol.NI^
HsO.
-^40
-30
—20
294.6
278.1
176.8
• • •
• • •
• • •
20
30
52.6
46.0
40. 3
710
635
595 (a*?
— 10
iii-S
• • •
35
35 5
0
87s
"99
40
307
5
775
1019
45
27.0
10
15
67.9
60.0
910
802
SO
S6
22.9
18.5
SoLUBiLrnr of Ammonia in Water Determined by Method op Lowering of
Freezing-Point.
(Rupert, 19x0.)
r
°«G^S: Solid Phu..
M Gms. NHaper
* xoo Gms. SoL
Solid Phase.
0
0 lee
-80.6 52
NHiH^
- 2
2
-82.8 54
If
- 4.6
4
-85.8- 56
f«
- 7.6
6
—87 Eutec. 56.5 N
H».Hi0+3NH^Hi
- 10.6
8
-84.8 58
aNHiH^
- 13-9
10
—82.2 60
(1
- 17.6
12
—80,4 62
M
- 21.4
14
-79.2 64
M
- 25.8
16
— 79.8 m. pt. 66
U
- 31.3
18
— 79.2 68
U
- 37
20
-80.3 70
M
- 43-6
22
—82.1 72
M
- SO-7
24
-84.5 74
M
- 60.3
26
-87.4 76
a
— 72.2
28
-90.4 78
M
- 87.2
30
—93.6 80
II
-102.3
32
—94 Eutec. 80.3
sNH^H^+NHi
— 116. 7
34
—91.7 82
NHi
— 120
EuteC. 34.5 Ice+NHiIM
> -89.4 84
M
-103.8
36 NHiHaO
-87.4 86
M
- 92.9
38
-85.6 88
M
- 86.7
40
—84.1 90
M
- 83.5
42
—82.7 92
M
- 81.4
44
-81. s 94
a
- 80
46
-80.3 96
M
- 79-3
48.7
-79.1 98
M
- 79-4
50
— 78 100
(•
More recent data on the above
system, by Smits and Postma (1914) an
in the region of the eutectic Ice + NHtHi<
quite doeely with the above except
These authors report a temperatun
e of —100.3 instead of —120 for this poir
Additional determinations are also given by Baum6 and Tykociner (1914). Older
data for the ice curve axe given by Guthne (1884) and Pickering (1893).
AMMONIA 34
Vapor Pressure of Aqueous Ammonia Solutions.
(Pennan, 1903.)
i.NHapet
Gns. SoL
Vapor Prssur in mm
. of Meicaiy at:
'o-.
lO*.
»•.
30*.
*>•.
so*.
6o*.
0
4-5
9
175
31 5
55
125
149-5
2-5
13
18
325
56-5
91
146
234
5
20
27
47-5
83
1345
210
327
75
275
40
70
"S
183-5
281
425
10
35
54
93
153 -5
241 -5
363-5
539-5
"•5
45
69
118
193 S
303-5
455
666
IS
57-5
89
151
245
377-5
564
816. s
17s
75
"5
191
305-5
465.5
688. s
985
20
93
144
237
393
569-5
834-5
II9I
22.5
117
180. s
291
455 S
690
1005
1432
25
1445
226.5
360
561 5
830.5
"95
• • •
27-S
181
280
440
680
1007
■ « •
• • ■
30
222
346
537
817
1189.5
• • •
• ■ •
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 r^;ular intervals of conceatratioa
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. PenoAH, J. Cbem. Soc. (Load.)* 81, 480, 1903.)
Vapor pressure determinations were made as above described on aqueous
solutions of the following compositions — (a) io.J.3% Urea -|- 16.36% NH|,
(W 5.29% Urea + 17.22% NH,, (c) 4.56% Mannitol -f 12.27% NH,, (d) 3.05%
Kj^4 + 7.49% NH,, (e) 5.27% NH4CI + 16.85% NH,, (/) 10.26% NrflCl
+ 12.9% NH,, {g) 2.68% CUSO4 -f 14.65% NH,, (h) 3.94% CUSO4 -f 6.54%
NH,.
The author's data were plotted on cross section paper and the following values
read from the curves.
t*. Vapor Presare of Eadi Solution in mm. of Mefcmy.
(a)
(»)
ic)
W
(•)
(f>
(0
W
20
204
200
120
• • •
193
130
iSS
• ■ •
30
325
3^S
198
• • «
302
320
235
87
40
48s
500
3"
200
471
34S
36s
145
so
71S
727
46s
304
695
522
545
223
60
1050
1060
70s
453
97S
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
AlfMONIA
Mutual Solubilitt of Aqubous Ammonia and Potassium Carbon-
ATB Solutions.
(Newth — J. Chem. Soc. 77f 776f zgoo.)
The solutions used were: Potassitim Carbonate satrirated at 25®
(contained 57.2 grams KsCO, per 100 cc). Aqueous Ammonia of
0.885 ^P- ^i*- (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.
SKtanted K«CX)!i in Aq. Ammonia.
cc KiCOftper
100 oc
DCH per %K^Cb Sohitiaii
Ammonia* m Auxtnre.
Aq. Ammonia in Sataiated KKX)!i.
cc. Ammonia %K«COs Soludon
in 100 cc. KfCOa. in Mixture.
I
6
zz
16
dz
26
31
38
39
42
43
a.o
30
S-o
6.S
10. s
20.0
31 .0
25 o
35 o
a.o
30
4-7
6.1
8.0
95
II. I
16.6
17.0
20.0
26.0
37 S
47 S
S^S
60.0
77 S
105.0
152.5
195.0
220.0
250.0
285.0
72.7
67.6
65.0
63 0
56-3
49.0
39 o
33 o
31 o
38.5
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 K>CO» Sohition in:
••. Ammonia KfCOs Sol.
Layer. Layer.
O 8 62 .
10 II 52
20 15 38
25 (crit. pt.) 25
With the addition of 12.9 percent 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.
(RaonltO
o
8
z6
a4
In Catdom Nitrate Solutiont
Gms.NHsper loo
Cms. Solvent in:
••• cMi. ^^^
96.25
78.50
65.00
104.5
84.7s
70.5
In Potaainm H
Gma.
Gma.
'iS
g?
72.0
57 o
46.0
37 3
The ffeezing-point curve for mixtures of ammAnia and ammonium thiocyanate
given by Bradley and Alexander (1912).
AlfMONIA
36
Solubility op Ammonia in Aqueous Salt Solutions at 25^
(Abegg and Riesenfeld, 190a.)
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 indiflFerent 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. HCl 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 odculate the solubility from the vapor pressures, it is only necessary to divide
the value for the molecular vapor pressure in HsO by that for the salt solution.
Thus the solubility of NH« in HsO 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. NH« per liter of the particular salt solution at
25^. In a later paper by Riesenfeld (1903), additional determinations are given
for 35^
Salt
M0IS.NH1
per Liter Salt Sol. of:
Salt
Mols. NH]
1 per Liter Salt Sol. of:
Solution.
0.5 n.
X n.
Z.5 n.
Solution.
0.5 n.
X n.
X.5 n.
KCl
0.930
0.866
0.809
KCN
0.926
0.858
0.802
KBr
0.950
0.904
0.857
KCNS
0.932
0.868
0.814
KI
0.970
0.942
0.900
KjSO*
0.87s
0.772
0.678
KOH
0.852
0.716
0.607
K2SQ,
0.865
0.768
0.675
NaCI
0.938
0.889
0.843
K2CO8
0.788
0.650
O.SS4
NaBr
0.965
0.916
0.890
K,C04
0.866
0.771
0.675
Nal
0-99S
0.992
0.985
KaCrO*
0.866
0.771
0.67s
NaOH
0.876
0.789
0.716
CHgCOOK
0.866
0.765
0.685
LiCI
0.980
1.008
1.045
HCOOK
0.868
0.760
0.678
LiBr
1. 001
1.040
1.090
KBO2
0.814
0.677
0.560
Lil
1.030
1.094
1. 190
K2HPO4
0.860
0.749
0.664
LiOH
0.863
0.808
0.768
Na^S
0.887
0.79s
0.726
KF
0.839
0.722
0.626
*KCIQa
0.927
...
• . .
KNOs
0.923
0.862
0.804
*KBiOs
0.940
...
• . •
KNO2
0.920
0.85s
0.798
♦KlOs
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 NH| in mm. of Hg., m = molecular concentra-
tions of NH| and n » molecular concentration of AgNOs. 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 AlfMONIA
Solubility op Ammonia in Absolute Ethyl Alcohol.
(Delepioe — J. pharm. chim. [5] 35* 40^ ^tSga; de Bruyn — Rec. trav. chim. zit zxa, '9a.)
Density.
Gros. NHs
per xoocc.
Solution.
Cms. NH3 per zoo
Gms. Sohition.
Cms. NHs pel
tDelepine.)
r 100 Cms. Alcok
t*.
(Ddepine.)
(de Bniyn.)
(de Biuyn.)
0
0-783
^3 OS
20.95
19.7
26.5
245
s
0.784
12.00
19. 00
17s
23.0
21.2
10
0.787
10.85
16.43
15.0
19.6
17.8
IS
0789
9.20
13 00
13.2
15.0
iS-3
ao
0791
7 SO
10.66
"•5
II. 9
13-2
as
0.794
6. CO
10. 0
10. 0
II .0
II. 2
30
0.798
S'^5
9-7
8.8
10.7
95
According to Mflller (1891), one volume of alcohol absorbs 340 volumes of
ammonia at 20*^ and 760 mm. pressure.
Solubility op Ammonia in Aqubous Ethyl Alcohol.
(Delepiiie.)
In 06%^ Alcohol. In 90% Alcohol. In 80% ^Alcohol.
^** Sp. Gr. G. NHs per Sp. Gr. G. NHs per Sp. Gr. G. NHs per
Solution, zoo Gms. Sol. Solutian. zoo Gms. Sol. Sdution. too Gms. Sol.
o 0.783 24.5 0.800 30.25 0.808 39.0
10 0.803 18.6 0.794 28.8 0.800 28.8
ao 0.788 14.8 0.795 ^5-^ 0.821 19. 1
30 0.791 10.7 0.796 II. 4 0.826 12.2
In 60% Alcohol. In 50%^ Alcohol.
••• Sp. Gr. G. NHs per Sp. Gr. G. NHs per
Solution, zoo Gms. Sol. Solution, zoo Gms. Sol.
o 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 op Ammonia in Absolute Methyl Alcohol.
(de Bruyn — Rec. trav. chim. zz. xxa, '92.)
^. G. NHs pw^ioo Grams. ^ G. NHs pcr^ xoo Grams.
^lution. Alcohol.
20 19.2 23.8
25 16.5 20.0
30 14.0 16.0
Solubility of Ammonia in Ethyl Ether.
(Chiistoff, z9za.)
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, pagje i) are given
by Bauml 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 Kuff and Geiaei (1906); results for ammonium and hydrogen sulfide
are given by Scheffer (1912).
Solubility of Ammonia in Hydroxylamine.
(de Bruyn, z89a.)
160 gms. of the sat. solution contain 26 gms. NHs at d=o^ and 19-20 gms. at
l5'*-i6^
» •
Solution.
Alcohol.
0
29 -3
41 5
5
26.5
36.4
10
24.2
31 B
IS
21.6
27.8
AlfMONIA
38
Distribution of Ammonia between:
Water and Amyl Alcohol at ao^
(Hen and Hadier — Her. 37i
4747. '04 )
Gnu.NHai>erzoocc. G.M.NHaPerioocc.
Water and Chloroform at 20®.
(Dawson and McCrae — J Ch. Soc. 70^ 496, 'ox; aee
also Hantsch and Sebaldt — Z. phys. Ch. 30, 358, '9^\
Aq.
Layer
Alcdiolic
Layer.
O
I
2
3
4
5
S
o
o
o
o
.0
072
147
272
438
595
0.756
o
o
o
o
Aq.
Layer.
0.25
050
1. 00
2. 00
3 00
Alcoholic
Layer.
0.003s
00073
0-0148
o 0295
0.0460
>■
CHCla'
Aq.
CHOi
Layer.
Layer.
Layer.
Layer.
0.2
0.007
O.OI
0. 00038
0.4
0015
0.02
0.00073
0.6
0023
0.03
000114
0.8
0031
0.04
0. 00152
I.O
0039
005
0.00193
1.2
0.046
0.06
0.00232
1-4
0.055
0.08
O.OO3II
1.6
0063
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), (1901a), (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. NHi per liter and only 10 when 12.23 gm. mols. NH| 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), (Daw^n, 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)i on the distribution at i8*
are given by Dawson (1909).
Results for the effect of ammonium rhromate 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.
(Hantach and Vagt, 190X.)
Cms. NHa per xoco cc
Mob. NHi per 1000 cc.
« .
CiHftCHi Layer.
Air.
C»H|CHa Layer.
Air.
0
0.366
0.0396
0.0215
0.00233
10
0.3S7
0.043s
0.0210
0.00256
20
0.326
0.0451
0.0192
0.00265
30
0.286
0.0462
0.0168
0.00272
39
AHMONIUM ACITATK
AMMONIUM ACETATE CH|C(X)NH4.
100 cc. of sat. solution in acetone contain 0.27 gm. CHsCOONHi at 19^
(Roshdestweoaky and Lewis, 19x2.)
AMMONIUM ARSENATES.
Thb System AMMomA^* -Arsbnic Trioxidb and Water at 30**.
(Schreinemaken and de Baat, 19x5.)
Gms. per xoo Gms. Sat. SoL
Gms. per xoo Gms. Sat. Sd.
NHi.
AsA.
ooua jrnaae.
NH,.
As,0,.
0
2.26
As^»
313
12.30
1. 41
10.98
ti
^•91
7.63
2.78
20.49
it
6.9s
4.72
2.86
21.17
tt
9-93
3.20
2.88
18.43
NH4ASQ,
4.28
2.16
SoUdPbaK.
NH4ASO1
u
ti
il
Data are also given for the system NH4CI -|- AssOa -|- HjO at 30®.
100 gms. HiO dissolve 0.02 gm. NH4CaAs04.iHsO.
" " " " 0.014 " NH4MgAs04.iHiO.
(Fidd, X873.)
SOLUBILrTY OF AMMONItm MAGNESIUM ARSENATE IN WaTER KSD IN
Aqueous Solutions op Ammonium Salts.
(Wenger, x9xx.)
Gins. NHiMgAsOi per xoo Gms. of Each Solvent.
r.
o
20
30
40
so
60
70
80
Water.
0.0339
0.0207
• . a
0.0275
0.0226
0.0210
0.0156
O-O236
nh^& ^ci!
0.092
0.114
0.118
0.139
0.189
0.211
0.189
0.189
0.084
0.113
0.113
0.190
0.189
0.219
0.221
0.231
Aq.*
NHiOH.
0.0087
0.0096
• • .
O.OII7
O.OIOO
0.0090
0.0095
0.0091
Aq.
NHiOHt
N&6.
Aq.
NHiOHf
+10%
NHiCI.
0.013 0.032
0.047 0.054
Solid Phase.
NHftBigAs0i.6Hy0
«
II
II
II
M
M
* Composed of x part NHi(<{ - o^) + 4 parts HiO.
t Contained 4 parts NHs(J '» 0.90) per xoo parts NHiCl solutioo.
AMMONIUM BENZOATE CsHsCOONH^.
Solubility in Water and in Aqueous Alcohol at 25**.
(Seidell, x9xo.)
Gma.CiEbOH
per 100 Gms.
Solvent.
O
10
20
30
40
SO
^ ol Sat. Sol.
1.043
1.027
1. 012
0.997
0.979
0.956
Gms.
CtHiC00NH4
per 100 Gms.
Sat. Sol.
18.6
18
18
18. 1
18
17
Gms. CtHsOH
per xoo Gms.
Solvent
60
70
80
90
95
100
dm of Sat. SoL
0.930
0.901
0.864
0.828
0.810
0.796
Gms.
CeH|COONH4
per xoo Gms.
Sat. Sol.
IS
12.2
8.3
2.7
1.6
100 gms. water dissolve 19.6 gms. CeHsCOONHi at 14'' 5, du of sat. sol. »
1X^2. (Greenish and Smith, x9ox.)
100 gms. water dissolve 83.33 pns. C«HjC(X)NH4 at b.-pt. (U. S. P.)
100 gms. glycerol dissolve 10 gms. C6HfCOONH4 at room temp. (Eager.)
AMMONIUM BORATES
40
The System Ammonia, Boric Acid
AND WaTI
CR AT 30®
AND AT 60®.
(Sborgi, 1913-15; Sboigi and Meccacd,
1916.)
Results at 30*.
Results at 60*.
Gms. per xoo
Gms. Sat. So
'' Solid Phase.
Gms. per 100 (
Sms. Sat. Sol.
Solid Phase.
(NH4)«0.
BsOi.
(NH4)«0.
BsOs.
0.23
4.81
HjBQa
0
7-39
HjBQ,
0.70
7.20
«
0.78
12.12
((
0.78
7.62
H8B08+ 1.5.8
1.42
15.60
HJBQ,+ 1.5.8
0.99
7-53
1.5.8
1.70
15-29
i.S-8
1.08
7.66
a
323
18.60
<(
1. 71
913
a
4.02
26.38
1.5.8-4-1.4.6
2.25
10.71
u
4.88
21.76
1.4.6
2.89
12.32
u
6.41
24.32
li
3-13
12.59
a
7.90
2731
1.4.6-4-1.2.4
3-43
6.35
2.4-5
7-83
26.76
1.2.4
6.51
448
«
7.91
17-57
((
10.4s
3-37
a
9-57
13.56
U
18.05
2.02
ti
15-45
8.33
a
24.80
151
a
19.47
5-92
a
30 56
1.22
u
22.57
4-47
ii
45-34
0.84
it
1.5.8 = (NH,),0.5B,Qs.8H«0
2.4.5 = 2(NH4)t0.4B,Qs.5HOi
1.4.6 » (NH4)i0.4B,0,.6HiO
1.2.4 = (NHi),0.2BiQs.4HiO
AMMONIUM BROMIDE NH4Br.
Solubility in Water.
(Smith and Eastlack, 1916.)
(Determinations by sealed tube method.)
Gms NfiUBr
Gms. NH4Br
Gms. NHiBr
r.
per zoo Gms.
f.
per 100 Gms.
f.
per xoo Gms.
HsO.
HiO.
HsO.
17 Eutec.
47-3
60
107.8
130
180
0
60.6
70
116. 8
137.3
Transition pt.
10
68
80
126
140
192.3
20
75-5
90
135-6
150
202.5
30
83.2
coo
145-6
160
213-4
40
91. 1
no
156.5
170
225.5
50
99.2
120
167.8
Solubility op Ammonium Bromide in Absolute Ethyl Alcohol,
Methyl Alcohol, and in Ether.
(Eder; de Bruyn— Z. phys. Ch. zo, 783. '93.)
In Ethyl Alcohol.
Gms. NH4Br
per 100 Grams.
••.
Solution.
AlcohoT.
IS
2.97
3.06
19
3.12
3.22
78
9-50
10.50
100 cc.
ethyl alcohol of dn
sat. sol. B
•• 0.8848.
In Methyl Alcohol.
Gms NH4Br
per 100 Grams.
Solution
Alcohol.
• • •
II. I
• • • •
• • •
"S
• • • .
In Ether (o 799 Sp. Gr.X
Gms. NH4Br
per xoo Grams.
Ether.
0.123
' 0.8352 dissolve 7.8 grams NH4Br at 15', dig of
(Greenish, 1900.)
100 CC. anhydrous hydrazine dissolve no gms. NH4Br at room temp, with
evolution of ammonia. (Welsh and Bioderson. 19x50
41
AHMONIUM BBOISIDE
SoLUBiLiry OF Ammonium Bromidb at 25"* in Mixtures of:
(Hen and Kohn, 1908.)
Methyl and Ethyl
Propyl and Methyl
Propyl and Ethyl
-
Alcohols.
Alcohols.
Alcohols.
t Gms.
CibOHpei
zoo Gms.
Solvent.
Gin.s.
Gtm.
riH,OHper iVof
xoo Cms. Sat. SoL
Solvent.
Cms.
Gms.
Gms.
iVof
Sat. SoL
NHiBr
per xoo
cc. Sat.
Sol.
NH«Br
per zoo
cc. Sat.
Sol.
CiHtOH
per zoo
Gms. Sol-
vent.
Sat. Sol.
NHiBr
perioo
ccSat.
Sol.
0
0.8065
2.5s
0 0.8605
9-83
0
0.8065
2.55
4.37
0.8083
2.99
II. II 0.8524
8.51
8.51
0.8062
2.51
10.40
O.8117
3.21
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
0.8501
8.13
91.8 0.8097
1.28
88.6
0.8042
I. II
84.77
0.8508
8.47
93-75 0.8089
I 25
91.2
0.8049
I. OS
91.25
0.8551
9.34
100 0.8059
0.95
95-2
0.8059
1.04
100
0.8605
9.83
100
0.8059
0.9s
AMMONIUM Cadmium BROMIDE (NH4)CdBr,.iHsO.
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, X876.)
AMMONIUM Platinum BROMIDE (NH4)2PtBre.
100 gms. sat. aqueous solution contain 0.59 gm. salt at 20^. (Halberstadt, Z884.)
Solubility of Tbtra Ethyl AMMONIUM BROMIDE N(CtHs)4Br, and of
Tbtra Methyl Ammonium Bromidb N(CH«)4Br in Acetonitrilb.
(Walden — Z. phys. Ch., 55, 7", '06.)
100 CC. sat. solution in CH«CN contain 9.59 gms. N(CiHs)4Br at 2<j^
100 cc. sat. solution in CHiCN contain 0.17 gm. N(CHi)4Br at 25 .
Solubility of Tbtra Ethyl Ammonium Bromidb in Water and
IN Chloroform at 25**.
(Peddle and Turner, X9X3.)
100 gms. HsO dissolve 279.5 S^is. N(CsH()4Br.
100 gms. CHCU dissolve 25.01 gms. N(C2H»)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)2CQt.
100 gms. HsO dissolve 25.4 gms. ammonium carbonate, calculated as
QHuNiOs at 16.7° d of sat. sol. = 1.095. (Greenish and Smith, xgox.)
100 gms. of carefully purified glycerol dissolve 20 gms. (NH4)iC0i at 15®.
(OsMndowski, 1907.)
AMMONIUM BIOARBONATE NH«HCO,.
Solubility in Water.
(Dibbits^ J. pr. Ch. [s] lo^ 417, '74.)
••• '
dtoM.'NHJRCO,
( per 100 Grams.
*•.
Grams NHiNCOy
Solution.
per xoo C
Solution.
Water:
Water:
0
10.6
II .9
20
17.4
21.0
5
12. 1
13-7
«S
19 3
«3-9
20
13-7
IS -8
30
ai-3
2J.O
«S
JSS
18.3
AHMONIUM BICABBONATI
42
Solubility op ammonium Bicarbonate in Aqueous Solutions op
Ammonium Chloride Saturated with CO,.
CFedodflff — Z. phjrt. Ch. 49^ t68, '04.)
O
o
IS
IS
IS
IS
IS
IS
IS
IS
IS
30
30
iccSoL
077
064
063
063
062
o^S
069
076
08s
08s
G.M.
Per xooo cc. Solotioa.
JV.I
Per tooo Gnmi B^.
G.M. Gms. Got. G.M. G.M. Gnw. Gmi.
NBA NHiHCO^ NH^. NH«HCO». NH«a. NH«HC0^ NH«a. NH«BOQ^
• • •
4.41
0.0
OS
I.O
1. 41
Z.89
2.87
3-84
4.82
4-9S
• ■ •
• • •
0.37
2.12
1.84
IS9
1.42
4.28
0.99
0.79
0.65
0.62
• • •
i • • •.
23s -9
0.0
26.8
S3S
7S-4
ICO. 8
IS3-3
205.2
2S7-9
264.8
29.3
167.2
I4S-2
112,2
lOI.I
78.2
62.5
SI -4
48.9
0.0
S-42
0.0
0.56
I 13
IS9
2.18
3-42
503
6.21
6.40
0.0
7-4
1.22
0.46
2 36
2.06
1.80
1.60
1.48
1. 18
0.98
0.84
0.81
3 42
I IS
0.0
290.8
0.0
29.9
60.6
85.1
116. 8
183.0
269.3
343 S
0.0
397 o
X19.0
36-0
186.4
162.9
142.2
126.9
116.8
93-3
77-3
66.4
64.2
270.0
91.0
Solubility op Ammonixtm Bicarbonate in Aqueous Solutions ov
Sodium Bicarbonatb Saturated with CO,.
(Fedodeff.)
TH'^ 'g.M. G.M. Gms.
Gms.
Ptt zooo Grams H^.
••.
G.M.
G.M.
Gms.
Gms.
z oc Sol. NaHCO^ NH«HC0^ NaHCO^ NH«HC0|. NaHCO^ NH«HC0^ NaHCO^
NH«HCO^
0
.*• .*• •••
• ■ •
• . •
0.0
I SI
0.0
119. 0
0
1.072 0.53 1.28
44.6
IOI.4
0.58
1-39
48.2
109.4
'S
1.064 0.0 2.12
0.0
167.2
0.0
2.36
0.0
186.4
IS
1.090 0.63 1.92
52.5
151-3
0.71
2.16
S9-2
170.6
30
••• ••• •••
• • •
• • •
0.0
3-42
0.0
270.0
30
••• ••• •••
• • •
• • •
0.83
2.91
70.0
230.0
SOLUBIUTT OF AMMONIUM BICARBONATE IN AqUBOUS SOLUTIONS OF
Ammonium Nitrate
*
(Fedotieff and Kottimoff, 19x4.)
r.
iofSat
Gms. per zoo Gms. IbO.
r.
dofSat
Gms. per zoo Gma. H^.
SoL
KH«NOb.
NH4HC0b.
SoL
NH«NOb.
NHiHCOk.
0
0
ZI.90
IS
Z.242
103.4
8.25
0
1.265
118
4.S2 •
IS
Z.269
Z28.9
7-79
IS
1.064
0
18.64
IS
1.302
Z66.9
7.46
IS
I.II3
23.26
12.91
30
• . •
0
26.96
IS
Z.Z64
49.82
10.33
30
• • •
231-9
12.57
43
AMMOKIUM BICARBONATE
Solubility of Mixtures op Ammonium Bicarbonate, Sodium
Bicarbonate, and Ammonium Chloride in Water
Saturated with CO,.
(Fedotieff.)
f. ,
m.of
ccSoL
Gram Mokjper
Gms-HsO.
1000
Cms. per xooo Gma. HsO.
Solid
NaHCOs. Naa.
NH4d.
^aHC09.
NaCl.
NH4a.
STuaaCm
O I
.114
0.59
0.96
4.93
49.61
56.16
263.4
a+b + C
O I
.187
O.I2
483
a
•74
10
.09
282.6
146.7
«
.116
093
0.51
6
.38
78
.18
29.84
336 a
((
.178
0.18
4.44
3
•73
15
13
259.8
199.6
u
151
030
3 09
4
56
25
.23
180.8
244.1
a + C
.128
051
1.68
S
45
42
.87
98.28
291.7
u
.112
0.99
0-35
S-
65
83
.22
20.47
302.4
a + b
.108
1. 07
0.20
5
21
89
95
11.70
278.9
(C
.106
1. 12
O.II
4
92
94
14
6.44
263.4
«
.101
1. 16
014
4'
00
97
52
8.19
214. 1
u
.090
093
0.95
3.
03
78
.18
55-58
108.6
tl
a-"
NaHCQ
i>.
b-
. NH,HCO„
c —
NH,CL
AMMONIUM Uranyl CARBONATE 2(NH4)sCOiUOiCC^
(Ebelmen.)
100 grams HsO dissolve 5 grams of the salt at 15°.^
AMMONIUM Lead COBALTICYANIDE NH4PbCo(CN)..3HiO.
(Schukr — SiU. Ber. K. Akad. W. (Berlin) 79. 3oa.)
100 grams HsO dissolve 12 grams of the salt at i8^.
AMMONIUM PerCHLORATE NH4CIO4.
Solubility in Water.
(Carlton, 19x0.)
r.
o
20
40
60
Sp. Gr.
Sat. S(d.
1.059
1.098
1. 128
1.158
(Sms. NH4a04
per xoooc.
Sat. Sol.
11.56
20.85
30-58
39 OS
r.
Sp. Gr.
Sat. Sol.
Gms. NH4Cia
per zoocc.
Sat. Sol.
80
II93
48.19
100
I. 216
57 01
107 b. pt.
1. 221
5912
In a paper by Thin and Cumming (1915), it is stated that ammonium per-
cUorate 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 E^s- NH4CIO4.
It 18 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 j.96 gms. NH4CIO4 per 100 gms. sat. solution, and
in 98.8 per cent alcohol containing 0.2 per cent HCIO4 gave 1.97 gms. per 100
gms. sat. solution.
AKHONinM PecCHLORATE
44
NH4CIO4
cm«i,cio«
(CH,)tNH,C104
CJtNHsClO*
(CJEl5),NH,C104
(CH,)»NHC104
(CH,)«NC104
(CtH»)4NC104
Cai»(CH,),NC10«
ICH,(CH,),NC10«
C»Hs(CH,),NC104
C,H7(CH,)>NC104
C4H,(CH,)^C104
C6Hu(CH,),Na04
Gms. Salt per
xoo Gms. HiO.
Solubility of Ammonium Perchloratb and Several of Its Derivativbs in
Water at 15°. (HofmuiQ» Httbald and Quoob (i9ix-za).)
Gms. Salt per
100 Gms. H|0.
CH,(CA),NC10« 43.6
CJH,(CiH6)sNC104 7.9
(CH,),(C,H6),NC104 134.3
CJI,(CH,),NC104 s
BrCA(CH,),Na04 3.5
BrC»H,(CHs),Na04 2.5
(0H)QH«(CH,),NC104 290.7
(0H)CH»CH(0H)CH,(CH,),NC104 155 . 7
NO,C8H4(CH,)JSrC104 0.6
CJI,(CH,),NC104 199. S
CH«(NH,C104)» 144. S
18. s
109.6
208.7
208.7
150.9
19.9
o-S
3-7
17.9
3-1
10.9
iS-4
3-7
2.2.
CH4[(CH,),NC104
C,H.[(CH,),NC104
Br,C»H,(CH,)JSrC104
1.2
i-S
3.2
2.6
BrCJEI,(CE,)J^C104
Mtlbauer (1913-13) found that 100 ems. of cold H|0 dissolve 1. 136 gm. tetra-
methyl ammonium perchlorate (CH|)«NCI04 and 100 gms. alcohol dissolve
0.04 gm. of the salt.
AHHOmUM CHLOBIDK NH«CL.
Solubility in Water.
(MuMer; bdow o°, Meerbiug — Z. uurg. Cb 31, ao}. 1903.)
f.
Gms. NH4CIJX
§olutioQ.
;r TOO Gms.
Water,
t«.
Gms. NH4C
1 per xoo
Gi
^udoa.
Water.
-IS
19.7
245
40
31 -4
45-8
— 10 9
20.3
25-5
SO
33 5
SO
4
-5-7
21.7
27.7
60
35-6
SS
3
0
22.7
29.4
70
37.6
60
2
+ S
23 8
31.2
80
39-6
65
.6
10
24.9
33-3
90
41.6
71
3
IS
26.0
35-2
100
43-6
77
3
ao
27.1
37-2
no
45-6
83
.8
25
28.2
39 3
115.6
46.6
87
3
30
29 -3
41.4
Density of saturated solution at o® = 1.088, at 15® = 1.077, at 19** = 1.075.
Eutectic, Ice -f NH4CI =* — 16® and 19.5 gms. NH4CI per 100 gms. sat. sol
100 gms. HfO dissolve 31.25 gms. NH4CI at 3.5^ 38.5 gms. at 25^* and 49.6
gms. at 50**. (Biltz and Marcus, X91X.)
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 COi. (FedoUeff — z. pi^yi. ch. 49, 169. 1904.)
Wt. of
I cc. SoL
Per 1000 cc. Solution.
Per xooo (
Qms. HjO.
t;
G. M. G. M. Gms. Gms. '
NH«HCOa. NH4CL NH«HCOs. NH«a.
G. M. G. M.
NH«HCO^ NH«a.
Gms. Gms.
NH«Ha. NH«a.
0
1.069
0.0 4.60 0.0 246.1
0.0 5.57
0.0 298.0
0
IS
IS
30
1.077
1.077
1.085
• • •
0.37 441 29.2 235.9
00 5.29 00 283.1
0.62 4.95 48.9 264.8
• •• ••« «■• ■••
0.46 5.42
00 6.64
0.81 6.40
00 7.78
36.0 290.8
00 3SSO
642 343 S
00 416.4
30
• • •
• •• ••• ••• •••
1. 15 7.40
91.0 397. <>
45
ABfMONIUM CHLOBIDS
Solubility in Aqubous Ammonia Solxttions at o^.
(Engel — BuIL soc. Ghim. I3] 6» 17, zSgi .)
Sp. Gr. of
Solotiont.
1.067
I 054
1. 031
1. 025
1. 017
0-993
0.992
0.983
0-9S3
0.931
MilUsnm Molecula
per 10 cc. SolutioQ.
Gmns'pear zoo cc.
Solution.
NHs.
S-37
12 .03
38.0
47 o
S4S
80.0
90.0
95-5
130.0
169.7s
NH«CI.
45-8
45
44
44
43
43
44
44
49
60
5
S
o
63
12
o
37
75
o
Kh«oh.
0.92
2.05
6.48
8.02
9.30
13 -66
15-36
16.29
22.18
28.97
NH«a.
24-52
2435
23.82
23-56
23 -35
23.09
23 56
23-75
26.63
32 14
Solubility of NH4CI in Aqueous Ammonia Solutions at 17.5^
(Stittmholm, 1908.)
Normality Eqmv. per lAcr. Gms. per looo cc. Solutk».
TraT NHiO. NH*. ' FnEcT
o 5.435 o 290.8
0.15 5.420 2.55 290
4.76 5.082 81 27Z.9
Solubilities op Mixtures op Ammonium Chloride and Other Salts
IN Water.
(RadorfF, Kaiaten, Mulder.)
Both salts present in solid phaaCi
19 5
21-5
20.0
18.5
150
22.0
Grams per 100 Gruns HtO.
Grams per 100 Grams BiiO.
29.2 NH^CIH- 174.0 NH4NO, R
26.8 " + 46.5(NHJ2S04R
33.8 " + ii.6BaCU R
39.2 " + i7.oBa(NOa), K
28.9 " + 16.9 KCl R
" + i9.iKa R
b.pt. 67.7 NH^ClH- 21.9 KCl M
14.8
18.5
14.0
18.7
18.7
38.8
39-8
36.8
37-9
22.9
+ 34.2E:N0,K
+ 38.6KNO,K
+ i4.iKjS04R
+ i3.3K,S04K
+ 23.9Naa R
30- 4 "
SOLOBom OP Ammonium Chloride in Aqueous S(h.utions op Ammonium
Sulfate at 30'.
(Wibaut, 1909; SchreinemaketB, 1910.)
Gms« per xoo Gms. Sat. Sol.
Gms. per 100 Cms. Sat. Sol.
(NH«),SO«
O
5
10
IS
20
NH«a.
295
28.5
257
23.2
20.2
Solid Phase.
NH4CI
tt
(t
(NH|),S04.
25
30
35
40
42
NH«a.
18.3
13-2
8.5
2.8
o
Solid Phase.
NH4Cl+(NH4)tS04
(NH4)2S04
€€
it
SoLUBiLiTT OP Mixtures op Ammonium Chloiude and Cobalt Chloridb
IN Water at 25'. *
(Foote. X9xa.)
Gms. per xoo Gms. Solid Residue.
Gns. per too Gms. Sat. ScL
NH«a.
17.90
13.59
8-75
7.45
7.62
CoCl^
15-63
25.19
34.28
35.24
34.61
NH«a.
83.01
3512
34.02
7.07
CoClf.
3-2
13.52
50.66
49.64
55-27
BW.
SoUd Phase.
Mixed ciystals of
3.47 [ NH4CI+C0CU.
14.22 1 2H2O
16.31 1 Mixed crystals +
37.66 I C0CI1.6H1O
JkMMONIUM CHLORIDE
46
SCH^UBILITY OF AllMONIUM CHLOKIDB IN AqUEOUS HYDROCHLORIC ACID.
Results at o^ (Engd. 1888.)
Sp. Gr. ol Sat. Gms. per 100 cc. sat. sol.
SoL
HCL
NHia.
1.076
0
24.61
Z.069
i.os
23.16
1.070
1.99
21.78
I 073
3-93
19.36
1.078
7.74
14. 54
1. 106
19.18
S.78
1. 114
22.07
4.67
Results at 25''
Gms-HOper
xoo Gms. H^.
O
0.91
1.82
3.6s
18.2s
(Annstrong mod Eyre, x9io-zx.)
dU Gms-NHfaper
Lt. SoL zoo Gms. Sat. SoL
Sat
1.080
1.079
1.082
1.083
1.099
28.3
27.4
26.4
24.6
"•3
Solubility of Mixture of Ammonium Chloride and Lead Chloride in
Water at Several Temperatures.
(At Z7*, 50* and loo* Deoiassieux (1913) at 35* Fooie and Levy, 1907.)
At I7'. At 25**. At 50*. At ICO*. Solid Phase
Gi08.'perzooGiiis.Sol. Gins.periooGins.Sd. Gms. per xoo Gms. Sol. Gmsj)erxooGms.Sol. in Each
Case.
fePbCU.
0.30
0.52
0.64
NH«C1.
27.03
26.68
26.49
PbCli. NH«a
1.20 28.15
Pba^
0.32
2.65
3-9^
NH«CL
34.14
33 62
33 56
0.34
0.098
0.078
0.078
0.076
0.16
0.21
0.89
22.32
12.36
4-93
4.23
3-48
1-43
0.96
o
0.93
0.3s
0.29
O.II
0.03
27.4s
21. S9
17.97
10. 25
2.77
3-31
1.76
0.71
0.49
0.48
0.67
1.08
1.69
31.90
27.16
19.42
12. 45
4.86
1.45
0.51
o
PbOt.
1. 61
4.21
• • •
9.26
9.88
11.60
12.67
11.40
8.32
4.54
1.98
1.76
1. 8s
2.02
3.10
NH4a
43.42 NHiQ
42.91 "
41.90
40.22
38.32
37.62
36.29
32.64
26.08
13.12
8.59
5.33
1.32
o
u
u
2.1
II
+a.x
" +x.a
t.a
11
M
II
"+pba,
PbCli
II
II
1.2 - NH4C1.2(PbCW, 2.1 - 2NH4CLPbCl,.
The following additional data for the above system at 22^ are given by BrOn«
sted (1909).
Gm. Equiv. Gm. Eqiiiv. PbOt
NHiQ per pei xoo Gms.
zoo Gms. H^. Sat. Sol.
O
O.Z
0.2
0.4
0.5
0.55
[0.6
0.7
7.49 Xio"
3.10 Xio"
1. 916X10'
1. 348 Xio"
1. 263 Xio"
1. 189X10"
1. 092X10"
0.956X10"
Solid Phase.
PbOi
II
M
II
II
aPbOt-NHia
11
Gm. Equiv.
NHiClper
zoo Gms. HfO.
0.8
I
2
3
4
5
6
Gm. Equiv. PbOt
per zoo Gms.
Sat. Sol.
O.837X1O-*
0.758XIO"*
0.695X10"^
0.968X10"^
1.502X10"*
2.338X10-^
3.580X10-*
SoUd Phase.
9PbaiJ<fHia
7. 29 sat. 6.46 Xio"
II
<i
II
II
M
W
<l
+NH«a
NThe two curves intersect at 0.52 normal NH4CI.
Solubility of Mixtures of Ammonium Chloride and Magnesium Chloride
IN Water. (BUtz and Marcus, 19x1.)
. . Gms. per xoo Gms. Sat . Sol.
SoUd Phase.
MgCl,. NH^a.
3.5 21.41 5.93 NH.a+Mga,.6H^
25 20.95 8.78
50 20.84 12.46 *"
f.
Gm.n. per xoo Gms. Sat. Sol.
Solid Phase.'
MgCI,. NH^a.
3.5 34.43 0.09 ^^^^^
25 35.41 0.09 "
50 36.92 CIS "
47
AMMONIUM CHLORIDS
Solubuxet op Mixhtsbs op Ammonium and Manganese Chloride^ ux
Water at 25^
(FooCe and Soxtoo, 19x4.)
ptf too Gms* Sttt. Sd.
NHdCL
23 -97
22.94
21.44
21.18
20.10
19.70
19 -75
19.67
Mud,.
7-97
9.6s
12.31
13.38
15.19
15.92
16.02
15.47
Solid Phaae.
Gms. per 100 Gms. Sat. Sol.
ayrtab
or and 0 mixed
oystals
NH«CL
17.09
15.05
13.17
9.15
5.90
3.77
2.98
2.94
MnClt.
18.76
22.44
24 52
29.24
34.78
39. 48 J
Solid Phue.
0 mixed crystals or
double salt aNHiO.
MnCltsH/)
43.71 1 aNILaMnCU.aIV)
43. 44 J +Mna,.a^ ,
a mixed crystals consist of NH4CI with varying amounts of MnCls.2HiO;
0 mixed crystals consist of the double salt 2NH4Cl.MnCl2.2HsO with excess of
NH4CI.
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*.
(Meerbuig, 1908.)
Gms. per too Gi
OS. Sat. Sol.
Solid
H«CV
NH«a
Phase.
0
29.50
NH«a
32.80
26.91
«
42-45
25 05
M
5005
24.79
« i.a-1
5308
22.77
X.3.1
58.90
20.02
" +X.X.I
56.38
18.50
Z.I.X
55-58
16.82
f<
57 -oi
14.12
" +3.a.i
56.26
13.04
3.3.x
Sms. pec 100 Gn
IS. Sat. Sol.
Solid
HgCt
NHiCl.'
Phase.
57-05
9.92
3.3.x
58-65
9.20
" +9.3
*Si-83
8.76
9.3
V
7.52
If
*35-6o
5.26
«
♦32.90
5.06
.1
29.65
362
" +Hga,
40.12
SI3
HgCl.
21
2.29
I(
7.67
0
M
1.2.1 = HgCl,.2NH4Cl.H,0: i.i.i - HgCl,.NH4Cl.H,0;
3.2.1 - 3HgCl,.2NH4Cl.H20; 92 - 9HgCl2.2NH4Cl.
* In these solutions 3 to 3 wedu were required for attainment of equilibrium.
SoLUBiLirT OP McrruRBs op Ammonium and Nickel Chlorides in Water
AT 25^
(Foote, X9Z3.)
Gns> per xoo Gms. Sat. SoL
NH«a
NiO,.
26.07
3.101
22.27
8.04
20.68
10.32
17.43
15.01
11.22
26.93
10.21
30.56
9.16
35.70 J
Sofid Phase.
Mixed crystals of
NILCland
NiOt-sHiQ
Gms. per xoo Gms. Sat SoL
NH«a.
7.98
8.07
8.23
8.17
.7.51
3.06
O
NiCli.
37
.41]
37
•73
37
•45
37
.64
37
.19
37
.98
37
■53]
Solid Phase.
Mixed crystals and
NiCl|.6HdO
NiClt.6H^
ammonium chloride 48
Solubility op Mixtures of Potassium Chloride and Ammonium
Chloride in Water at 25°.
(Fock — Z. Kryst Min. 38» 353, '97-)
Grams per liter
SolutioD.
Mol. percent
in SoiutioD.
Sp. Gr. of
CrJiiflrBia
Mol.
Soli
per cent to
d Phaae.
'Niua.
KCi.
NHiO.
KQ.
Uh^,
KcL
0.00
3" -3
0.00
100. 0
I. 1807
0.0
100
32.81
293 -3
9.41
90.59
I. 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
11591
6.18
93.82
127.8
234.6
46.59
53-44
1.1493
8.90
91.10
147-2
204.2
51-63
48.37
1.1461
10.53
89.47
197 -3
157.7
63.56
36.44
1-1391
17.86
82.14
232.5
116.8
73-49
26.51
I. 1326
60.20
39.80
2445
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
Z.I212
97-79
2. 21
278.6
53-16
87.96
12.04
I.ZOO9
98.85
I. IS
320.7
31 24
93-45
6.55
1. 0912
99-33
0.67
273 5
coo
xoo.oo
coo
Z.O768
100 .0
O»00
The following additional data for the above system are given by Biltz and
Marcus (191 1). The results show that NH4CI + KCl form a series of mix-
crystals broken by a gap which eictends between about 20 and 98 mol. per cent
NH4CI in the crystals.
Composition
of Sat. Solution.
Composil
ion of Solid Phase.
Cms. per
xooGms.
Sol.
Mols. per xooo Mola.
Gnu. per loo Gma.
Crystals.
Mol. %
NHiQin
NH«a.
KCL
NHiCl.
KCl.^
NH«C1.
Ka. '
Ci^rtala.
5.13
22.29
23.8
74.2
1. 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. II
65.9
55.5
5.89
94.11
8
15.46
14. S3
74.4
50.2
7.24
92.76
9.8
19-54
12.16
96.3
43
11.20
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
118. 2
22.6
98.28
1.72
98.8
These authors also give data for the ammonium chloride camellite and
potassium chloride camellite diagram at 25^.
Solubility of Mixtures of Ammonium and Potassium Chlorides in Water
AT 25**, 65* AND 90*.
(Uyeda, 191 a.)
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 CHLORIDS
Solubility op Ammonium Chloride in Aqueous Solutions or
Sodium Chloride Saturated with CO,.
(Fedodeff.)
Wt.cl
Per 1000 cc. Sohitiao
•
Per 1000
Gma. HaO
Gms.
»
••.
G. M.
G. M.
Gms.
Cms.
g.m.
G.M.
Gnu.
locSoL
Naa.
NH4CI.
Naa.
NH«a.
Naa.
NH«a.
Naa.
NH«a.
0
1.069
0.0
4.60
0.0
246.1
0.0
5-57
0.0
298.0
0
^8S
4.04
2.26
236.5
121 .0
4.89
2.73
286.4
146. 1
IS
077
0.0
5 29
0.0
283.1
0.0
6.64
0.0
355 0
IS
097
0.81
4.71
47 S
252.1
1.02
5-91
59-8
316.4
IS
I30
1.68
413
98.0
221.7
2.09
518
122.4
277.0
15
153
2.87
3 38
168.0
180.7
357
4.20
208.9
224.7
15
175
3-65
2.98
"3 5
159-4
4-55
3 72
266.8
198.8
30
* • •
• • .
. ■ •
• • •
• • •
0.0
7.78
0.0
416.4
30
I
.166
3.30
3 70
193.0
198.0
4.26
4-77
249.0
4S
» • •
• • •
• • •
• • •
M m •
0.0
9 03
0.0
483 -7
4S
» • •
• • •
• • •
• • •
• • •
4.0
6.02
233 -9
332.1
SoLUBiLiTT OP Ammonium Chloride in Aqueous Ethyl Alcoh(»< at 15^ and
AT 30®.
Gms.CApHper
100 Gnu. Sdvent.
ums. i^ii4Ui per j
00 vrnB. ooivrai ai;
'
,
IS .
30 .
0
35.2
40.4
20
25
29.7
40
16.8
19
60
95
II. I
80
4
S-3
92.3
1-3
• • •
100
0.6
• • •
Results at 15** by interpolation from Gerardin (1865), Greenish (1900) and
deBniyn (1892). Those at 30'' from Bathrick (1896).
100 gms. absolute methyl alcohol dissolve 3.35 gms. NH4CI at 19^.
(deBruyn, xSga.)
100 gms. 98% methyl alcohol dissolve 3.52 gms. NH4CI at I9.5^
(deBruyn, 1892.)
Solubility op Ammonium Chloride in Mixtures op Several Alcohols
WITH Water.
CArmstxong, Eyre, Hiiaaey and Paddington (1907); and Armstrong and Eyre Cz9x<h-zz.)
*•
Gm. Mols. Al-
Gma-NUiO
per xoo Gma. Sat. Solutioi
lin:
K .
Gms. H«0.
Aq. CHaOH.
Aq.C«Hf0H.
Aq. C,H|OH.
0
0
23
23
23
0
0.2s
22.8
22.6
22.7
0
0.50
22.6
22.2
22.3
0
X
22.1
21.5
21. 1
0
3
20.5
^9
• . •
25
0
28.3
28.13 (1.0805)
28.3
25
0.25
28.1
28 (1.0780)
28.1
25
0.50
27.9
27.6 (1.0753)
27s
25
I
27.6
27 (1.0704)
36.6
25
3
26.1
26.5 (1.0528)
• • •
25
5
• • •
22.6 (1.0376)
• • •
(Figures in parentheses show Sp. Or. of sat. sols.)
AMMONIUM CHLORIDE
SO
SOLUBILITT OF AMMONIUM ChLORIDB IN SEVERAL ALCOHOL MiXTUBBS AT 2^*
(Hen and Kuhn, 1908.)
In Methyl and Ethyl In Methyl and Propyl In Propyl and Ethyl
Alcohol. .^cohol. AIcohoL
Gm^. CH/)H
per 100 Gms.
Solvent.
Gms. NH,a per
100 Gbis. Sat.
Solution.
Gms. CaHfOH
per 100 Gms.
Solvent.
GmA. NH^Cl per
100 Gms. Sat.
Solution.
Gms. CsHiOH
per xoo Gms.
Solvent.
Gffis.NH4Cf
per 100 Gms.
Sat. Sdadan.
0
0.53
0
2.76
0
O.S3
ID
0.67
10
2.33
10
0.50
30
0.80
20
1.90
20
0.47
30
40
0.98
I. 18
30
40
1.58
1.26
30
40
0.42
0.39
so
60
1.40
1.6s
SO
60
I 03
0.82
SO
60
0.36
0.32
70
80
1.92
2.18
70
80
0.60
0.41
70
80
0.30
0.26
90
100
2.48
2.76
90
ICO
0.30
0.18
90
100
0.22
0.18
Solubility of Ammonium Chloridb in Aqueous Glycerol Solutions and
IN Aqueous Acetone Solutions at 25**.
(Hen and Knoch — Z. anoig. Chem. 45* 363, 367, '05.)
In Aqueous GlyceroL
(Sp. Gr.*of Glycerine 1.355, Imparity about x.5%*)
Wt.%
Glyoerme.
NH4CI per xoo cc.
Solution.
O
13
25
45
54
83
100
38
98
36
23
84
00
Millimols.
585 I
544-6
502.9
434-4
403 -5
291.4
228.4
Grams.
31-32
29.16
26.93
23.26
21.60
15.60
12.23
Sp. Gr.
at i^.
at ^o
Vol.%
in Aqueous Acetone.
S Ition.
NH«a per 100 oc.
Sp. Gr.
I
I
I
I
I
I
I
0793
0947
II27
1452
1606
2225
2617
O
10
20
30
40
♦46.5
*8s-7
90
L
U
MiIttmoh»
585 I
534 -I
464.6
396.7
328.5
283.7
18.9
9.4
Grams.
31
28
24
21
15
I
O
59
87
23
59
19
01
SO
I .0793
r.o6i8
I 0451
1 .0263
0.9998
0.9800
0.8390
0.8274
L indicates
* Between these two concentrations of acetone, the soltttioo separates into two layers,
lower layer, U indicates upper layer.
100 CC. anhydrous hydrazine dissolve 75 gms. NH4CI at room temp, with
evolution of ammonia. (Welsh and Brodeison, 19x5.)
Solubility of Tetra Ethyl AMMONIUM CHLORIDE N(CiH6)4Q, and
ALSO of Tetra Methyl Ammonium Chloride N(CHj)4Cl in Acetonitrile.
100 cc. sat. solution in CHgCN contain 29.31 gms. N(C2H6)4Cl at 25".
100 cc. sat. solution in CH3CN contain 0.265 gms. N(CH3)4C1 at 25 .
(Walden — Z. physik. Chem. 55, 713, '06.)
Solubility of Tetra Ethyl Ammonium (Chloride in Water and in
Chloroform.
(Peddle and Tamer, 19 13.)
100 gms. H2O dissolve 141. o gms. N(C2H5)4C1 at 25**.
100 gms. CHCU dissolve 8.24 gms. N(C2H8)4C1 at 25".
Solubility of Dimethyl AMMONIUM CHLORIDE in Water and in
Chloroform.
(Hantzsch, 1902.)
100 gms. HsO dissolve 208 gms. of the salt.
100 gms. CHCU dissolve 26.9 gms. of the salt (temp, not stated in abstract).
51
AMMONIUM CHBOBCATE
AMMONIUM OHBOMATEB.
Solubility in Water at 30**.
(Schreinemaker — 2L physic. Cfaem. 55, 89, '06O
Compoeidoa in Wt. per cent of:
The Snlmtion.
The Ra!4tie.
SaHd Phase.
%CKV
%NH,.
%CrO,.
%NH,.
6-933
22-35
• . •
• . •
(im,)jCtOt
9
966
16-53
47
•59
20.44
If
16.
973
8.20
•
» •
• • •
11
22.
S3
6-37
38
•03
12.15
it
27.
09
6.87
48
02
12.01
(NH«)^0«+ (NH«).Cr,0,
26.
19
5 -70
47
•38
8.81
(NH,)/:r,0,
25
99
S-io
41
•56
758
(t
30
.16
3 50
•
• •
• ■ •
tc
38
.89
3-IO
61
.08
8.80
' it
42
44
3-15
59
•72
6.7s
(NH4),Cr,0,-^(NH4),CrAu
44
.08
2.27
54
.90
4.14
(NH4).Cr/)..
52
.91
I. II
60
.88
3-09
«
54
56
1.03
63
.07
3 09
(NH4),Cr.O„-f (NH,).Cr40»
56
•57
0.97
65
.70
2.95
(NHO^^O,
58
87
0.65
69
74
3 24
it
62
.48
0.46
71
93
3.10
tt
63
.60
0.40
73
.68
1. 18
(NIC),Cr40i,+ CrO,
63
.66
0.41
71'
47
2.07
tt
62
94
0.2I
• f
•
• • •
CrO,
62
.28
O-O
• «
•
• • •
CrO.
100 gms. of the sat. aq, solution contain 28.80 gms.(NH4)aCr04 at 30®.
zoo gms. of the sat. aq. solution contain 32.05 gms. (NHJaCraOy at ^o\
AMMONIUM CITBATES.
Solubility in Aqueous Solutions of Citric Acid at 30*.
(van Itallie, 1908.)
(Data read from curve plotted from original results.)
Gms. per 100 Gms. Sat. Sol.
CVHO,.
NH|.
-. Solid Phase. -
CAO>-
NH,.
-> SoUdPbase.
65
0
CAOi.HiO
..S3
7-5
CAOiJ^
68
o-S
«
56
8.2
w
72
1-3
<f
59-1
8.5
CHANU4+CA0r(NH|),
75
2.3 <
r^HA-HsO+CsHA-NHi
54
8.5
C.iV)»(Nli4)s
70
2.4
C«H70r.NH4
50
7-9
u
6S
2-5
i(
45-8
8.4
M
60
2.7
u
47
II. I
M
55
52
2.8
2.8
M
a
50
54-5
12.9
145
<=*W^4&«^
50
3-6
tt
52
15
CtH.0)(Nli4)t.?H^
49.2
S-i
w
50
16
If
50
6.2
If
48.4
17.9
M
Composition of the solid phases determined by "Rest Method."
(Schreinemakers, Z. anoi^g. Ch. i7, 907*)
AMMONIUM CALCIUM FEBBOCYANIDE.
100 gms. sat. aqueous solution contain 0.258 gm. (NH4)2CaFe(CN)e at i6'.
(Bnmn.)
AMMONIUM FLUOBOBIDE NH43BF<.
100 parts of water dissolve 25 parts salt at 16®, and about 97 parts at b. pt*'
(Stelba — Chem. Techn. Cent. Anz. 7. 459 )
AMMONIUM FOBMATE
52
AMMONIUM FOBMATE HCOONH4, and also Ammonium Acid Formate.
Solubility in Water.
(Groschu£f — Ber. 36, 4351, '03.)
Gm
a.HCOONH
4perxooGi
ns- SoUd
■" Phase.
Gms. per loo Gms. Solut
»on. SoUd
• ■ <"■
Solution.
Water.
• HCOONH,.
HCOOH.
■" Phase.
— 20
41.9
72
HCOONHi
- 6.S 46.7
34.1
HCOONH«.HCOOH
0
50.5
102
«
+ 1.5 49-6
36.2
(C
20
58.9
143
u
6 SI -3
37-4
M
40
67.1
204
u
8.5 52. I
38
1*
60
75-7
3"
t€
- 7 49.6
36.2
HCOONU4 labil.
80
84.2
S3I
M
+13 S3
38.6
stabfl.
116 m.
.pt.
29 55-8
39 S7-8
40.7
42.2
U it
H^ free solutina
Solubility op Ammonium Formate in Formic Acid Solutions.
(Groschuff.)
^o grams of HCC)0NH4 dissolved in weighed amounts of anhydrous formic
acid and CQoled to the point at which a solid phase separated.
f.
- 3
+ 8.5
21.5
Gms. G. M.
HC00NH« HCOONHj Solid
per 100 Gms. per 100 G. M. Phase.
HCOOH.
Sdution.
35-3
40.6
SO
39-9
49-9
73 •
HCOONH*.
HCOOH
«
a
II
39
78
Gms. G. M.
HCOONH«. HCOONIL Solid
per xoo Gms.periooG.M. Phase.
Solution.
SO
57. 8
731
HCOOH.
73 HCOONH4 hJtuL
100
199
00
stabiL
116 m. pL 100
100 gms. 95% Formic Acid dissolve 6.2 gms. HCC)0NH4 at 21"
AMMONIUM lODATE NH4lO<.
Solubility in Aqueous Iodic Acid at 30®.
(Meerburg, 1905.)
u
t<
M
M
(Aschan, 1913.)
Gms. per 100 Gms. Sat. Sol.
mo,.
O
2.S4
4.52
6.S7
NH4IO1.
4.20
3.89
3 83
1.94
Solid Phase.
NH«IOk
Gms. per 100 Gms. Sat. Sol.
((
K
+NH«IQ,.aHIQ,
NH|I0,.2HI0.
HIOi.
24
44.43
76.3s
76.70
NHiIO,.
0.62
039
0.31
o
Solid Phase.
NHiIOs-aHIQ,
if
" +H10i
mok
(Baxker, 1908.)
AMMONIUM PerlODATE NH4IO4.
100 gms. HjO dissolve 2.7 gms. salt at 16*, du = 1.078.
AMMONIUM IODIDE NH4I.
Solubility in Water. Solubility in Aqueous Alcohol at 25*.
(Smith and Eastlack, 19 16.)
(Seidell, unpublished.)
^r
f
Gms. NHtl
per xoo Gms.
r.
Gms.NH4l
per 100 Gms.
Gms.CtHiOH . ^
per xoo Gms. «*?•«.
Gms. NHiIper 100 Gms
H,0.
HjO.
Solvent.
dai. doi.
Sat. Sol.
Solvent.
-27.5
Eutec. 125.2
40
190. s
0
1.646
64. s
181. 9
— 20
136
SO
199.6
10
I.S90
61.7
161. 1
— 10
I4S
60
208.9
20
I.S2S
S8.7
142. 1
0
IS4.2
70
218.7
30
1.462
ss-s
124.8
10
163.2
80
228.8
40
1.39s
52
108.3
IS
167.8
100
2SO.3
SO
1.320
48
92.3
20
172.3
120
273.6
60
1.250
43.8
77.9
2S
176.8
140
299.2
70
1. 168
39
64
30
181 .4
80
1.094
33-3
49.9
90
1. 013
27. S
37.9
ICO
0.929
20.8
.26.3
53
Tecra Ethyl AlOfONIUM IODIDE N(CsH.)4l.
AMMONIUM IODIDE
Solubility in Sbvbral Solvents.
(Walden — Z. physik. Chem. 55. 698, '06.)
Solvent.
Water
Water
Methyl Alcohol
Methyl Alcohol
Ethyl Alcohol
Ethyl Alcohol
Glycol
Glycol
Acetonitrile
Acetonitrile
Piopionitrile
PrapioDitrile
Benzonitrile
Methyl Sulphocyanide
Ethyl Sulphocyanide
Nitro Methane
Nitro Methane
Nitroso Dimethyline
Acetyl Acetone
Fuifuiol
Furfurol
Benzaldehyde
Salicylaldehyde
Anisaldehyde
Acetone
Acetone
Ethyl Acetate
Ethyl Nitrate
Benzoyl Ethyl Acetate
Dimethyl Malonate
Methyl Cyan Acetate
Methyl Cyan Acetate
Ethyl Cyan Acetate
Ethyl Cyan Acetate
Nitrobenzene
Acetophenone
Amyl Alcohol
Paraldehyde
Methyl Formate
Biomobenzene
o
25
o
25
o
25
o
25
o
25
o
25
25
25
25
o
25,
25
25
o
25
25
25
25
o
25
25
25
C6H6COCH2COOC2H5 25
CHs(C00CH,)2 25
CHjCNCOOCHs o
CHjCNGOOCH, .25
CHiCNCOOCsHfi o
CHsCNCOOCJIi 25
GHsNO, 25
CeEUCOCH,
CbHuOH
(C2H4O),
HCOOCH,
CsHftBr
(Walden
FonnuUt.
H,0
CHK)H
CH3OH
CaHfiOH
CaHjOH
(CH1OH),
(CH1OH),
CH3CN
CHjCN
CUCHjCN
CUCHjCN
CeHfiCN
CH3SCN
CjHiSCN
CH3NO,
CHaNOa
(CH3)2N.NO
CHaCOCHjCOCH,
CJty^.COH
CJIsO.COH
CeHfiCOH
CrfI4.OH.COH
C(a.OCH,.COH
(CH,)2C0
(CH,)2C0
CH,C00C,H8
C2H60N02
Sp. Gr. Gms. mCJSfjJ.
of « . .
Soltttion. cc- Solut](»x.
1.0470 16.31
I.I02I 36.33 (355)
0.8326 3-7-4-3
0.8463 10.5 (10.7)
0.7928 0.348
0.7844 0.98(0.88)
I. 1039 3.27
1.0904 7.63(7.55)
0.8163 2.24
0.7929 2.97(3.54)
0.8059 0.618
0.7830 0.81-1.01
0.467
1.0828 4.40
I. 0012 0.475
I. 1658 #3.59
I. 1476 5.38-6.27
2.67
0.268
3.91
5-33
0.43
change-
able-! 7. 7
0.59
0.174
0.249
0.00039
1.0984 0.062
I. 1303 0.321
0.040
1.82
2.83
1.057
1. 71
0.504
0.13
0.071
0.036
0.031
0.009
— Z. physik. Chem. 61, 635,
per 100.
^.0059
• » •
I . 1738
I. 1692
Gms.
Solution.
15.58
32.9
4.44
12.29
0.439
1. 113
2.97
7
2.74
3-74
0.767
0.99
0.451
4.06
0.47
3.004
4.72
2.66
• • •
3.33
4.55
0.7991
I . 1335
I . 1341
• • •
1.0760
1.0607
0.218
0.316
• • •
0.056
0.284
0.035
1.605
• • •
0.981
1. 41
0.422
0.127
0.089
0.037
0.032
0.006
i9or-'o8.)
AMMONIUM lODIDB
54
Tetra Methyl AMMONIUM IODIDE N(CH,)J.
Solubility in Several Solvents.
(Walden — Z. physak. Chem. 55* 708. '06.)
FonnuU.
»•.
Sp. Gr. o(
Solutiaa.
Gms. N(CH9)« 1
[ per xoo.
SoltVMt.
cc. Solutioa.
Gms.
Sdutiaa.
Water
H,0
0
1. 0188
2.01
1.97
Water
H,0
25
I .0155
5 -31-5 -89
5.22
Methyl Alcohol
CH,OH
0
0.8025
0. 18-0.22
0.22
Methyl Alcohol
CH,OH
25
0 ■ 7930
0.38-0.42
0.48
Ethyl Alcohol
CJH.OH
25
0.7894
009
■ • •
Glycol
(CH.OH).
0
• • •
1. 014
• • •
Glycol
(CHK)H).
25
1.0678
0.240
0.224
Acetonitril
CH.CN
25
• ■ •
0.650
• • •
Nitro Methane
CHJJO,
0
1.1387
o.?s-o.32
0.22
Nitro Methane
CHJJO,
25
I. 1285
0.34-0-38
0.21
Acetone
(CH,).CO •
0
• • •
O.I 18
• • ■
Acetone
(CH.).CO
25
• ■ •
0.187
• • •
Salicyl Aldehyde
CJI4.OH.COH
0
I . 1493
0.302
0.263
Salicyl Aldehyde
C34.OH.COH
25
I 1379
0.510
0.484
Very exact determinations of the solubility of tetra methyl ammonium iodide
in aqueous solutions of KOH and of NHiOH at 25® are given by Hill (19 17).
Tetra Propyl AMMONIUM IODIDE N(C,H7)4l.
Solubility in Several Solvents,
(Wftlden — Z. pbysik. Chem. 55. 709, '06.)
„ „ , Gms. N(CaH7)4l per 100.
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
Ethylnitrite
Dimethyl Malonate
Dimethyl Malonate
Acetone
Acetone
Ethyl Acetate
Ethyl Bromide
Fonnubu
r.
op. ur. Qi
Solution.
cc. Solution
Gms.
Solution.
CHiOH
0
0.9756
40.92
41.94
CHiOH
25
I. 0187
56.42
55-37
QHsOH
0
0.8349
6.5-6.8
8.14
CJthOH.
25
0.8716
19.88-20.
29 23.28
CH^N
0
0.8553
13 03
15 24
CH,CN
25
0.8584
18.69
21.77
COIsCN
0
0.8280
6.37
7.66
CiHsCN
25
O.8I9I
965
10.29
Cai«CN
25
I. 0199
8.44
8-35
CH*NOj
0
I. 181
14.79
12.52
CHJJO.
25
I. 158
22.24
19.21
QHsNOj
25
I 193
5-71
4 79
CHsCOH
0
I. 0581
7.06
6.67
QflsCOH
25
I .0549
9.87
9-35
C«H6.0CH,.C0H
0
I.III4
5.60
504
C«H6.0CH,.C0H
25
I. 1004
6.7s
6.14
C«Hs.0H.C0H
25
• • •
39.28
• • •
CjHsNO.
c
I. 1207
0.522
0.466
cjEWsro.
25
I . 1025
0.653
0.592
CH2(C00CH,)j
0
I 1532
0.298
0.259
CHj(C00CH,)j
25
I 1345
0.320
0.282
(CH,),CO
0
0.8259
2.692
4.65
(CH,),CO
25
0.8049
3-944
4.90
CHjCOGOHs
25
0S975
0.0063
0.007
QHjBr
25
• • •
• • •
0.187
(Walden — Z. physOc Chem. 6i, 639, igoT-'oS )
55
AMMONIUM IODIDE
Solubility of Tbtra Amyl, Tetra Ethyl and Tetra a Propyl Ammonium
Iodides in Water and in Chloroform at 25^. (Peddle and rumer. 19x3.)
Solvent.
Gzns. Each Salt (Determined Separately), per zoo Gms. Solvent.
N(CH,04l. N(C,Hi)4l. aN(C,H7)J.
Water 0.74 45 18.64
CHCI3 210.8 i.ss 5456
FriKzing'point data for mixtures of tetra methyl ammonium iodide and iodine,
and tor phenyltrimethyl ammonium iodide and iodine are given by Olivari (1908).
AMMOKIUM Iridium CHLORIDES.
Solubility in Water at 19^. (Deiepme, 190S.)
Name of Salt. Fonnula. ,00 toi.^.
Ammonium iridium chloride (NH4)»IrCl6 0.77
Diammonium aquo penta chloro iridite IrCl6(H20)(NHi)s 15 .4
Triammoniiun hexa chloro iridite IrCl«(NH4)8+H20 10.5
AMMONIUM lodo MEBCURATE 2NH4l.Hgl2.H,0.
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)20.4MoQi.2H20.
salt at 15" {d = 1.03), 3.67 gms. at 18** (d -
(Weibpe, 19x2.)
ICO gms. H«0 dissolve j.52 gms. sail
1x14) 2^d 4.60 gms. at 32^ {d = 1.05).
AMMONIUM Phospho MOLYBDATE (NH4)iP04.i4MoO<4H20.
Solubility in Water and Aqueous Solutions at 15**. (de LuccW, x9xo.)
Solvent. Gms. Salt per looo Gms. Sohrent.
Water 0.238
5 per cent aqueous NH4NQ8 solution o. 137
I per cent aqueous HNQs solution o. 203
AMMONIUM NITRATE NH4NO,.
Solubility in Water.
(Sdniuz — Oitwald's Lefarbuch, ad ed. p. 4a<; MoUcr and Kawfmann — Z. ph^ik. Cheni:
43, 497» oi-'oa.)
Gms. NHfN(Da per
j,jDer 100 (5ms.
Sp. Gr.
G.Mob.
NH«NOs
100 Mob.
O
12.2
20.2
aS-o
30.0
32.1
35 o
40.0
50. o
60.0
70.0
80.0
90.0
100 .0
1-2945
1.3116
1-3197
1 .3299
1-3344
I -3394
1.3464
26
34
43
48
54
57
59
66
77
94
112
130
166
196
63
54-
■so
60.
•30
65-
.19
68.
.40
70.
.60
71-
.80
72.
.80
74-
.41
77-
•73
80.
•30
83-
•50
85-
•50
88.
■00
89.
utxm.
19
53
80
17
73
97
64
82
49
81
32
25
08
71
Solid
Phase.
u
a
u
It
Water.
1x8 .3 NH4NO, rhomb, fi
1534
192.4
214.2
241.8
256.9 NH4NOS rhomb, fi + rhomb, a
265 .8 NH^NO, rhomb. «
297.0
344 o •
421.0
499.0
580.0
740.0 NHiNOsrhombohedral?
871.0
It
ti
it
u
ti
«
SOLUDILmES OF MIXTURES OF AMMONIUM NiTRATB AND OTHER SALTS.
(ROdorf— Mulder.)
100 gms. HsO dissolve 162.9 gms- NH4NO1 + 77.1 gms. NaNOs at 16° R.
100 gms. HjO dissolve 88.8 gms. NH4N0j + 40.6 gms. KNO» at 9** M.
100 gms. HiO dissolve 101.3 gms. NH^NOi -j- 6.2 gms. Ba(N08)2 at 9° M.
AMMONIUM NITRATE
56
80
60
44
30
10. S
o
-445
Solubility of Ammonium Nitratb in Ammonia.
(Knrikff — Z. phyiic. Cbem. as. 109, '98.)
NH«NO|.
O
I -3918
0.9526
0.8308
0.967s
0.7600
Gms.
NHt.
100
4-4327
1-2457
0.3700
03515
0.3607
Mol8.NH«NOa
per 100 Mola.
0.0
6.25
13 9
36 -9
383
33-3
35-9
68.8
94 o
190.8
168.0
Gnu.
MHcNO^
0-9358
o . 7746
4.2615
0.6439
0.7578
Mob
Gms. per 100
o 2352
o . 1857
0.7747
0.0665
0.0588
NH4N0a
+ NH^
4^9
4f o
53-8
67 -3
74.2
100. o
t° — temperattire of equilibrium between solution and solid phase
Solubility of Ammonium Nitratb in Aqueous Solutions of Ammonium
Sulfate and Vice Versa.
(Masamik, 19x6, xgx?.)
Results at o^
Results at 30**.
Results at 70®.
(de Waal. 1910.)
(Schrrfnemskers and Haenen, 19x0.)
(de Waal. 19x0.)
Gms. per
100 Gms. &t. Sol. SoKdPhMe. .
NH«NQ, ^^*
Gms. per
100 Gms. Sat. Sol. _ „ . _.
.____ . wwuu « ■■■■■' •
NH«N0i. ^^«
Gms.
xooGms.
^^ SoBdPhoe.
nh«nq,.
(NHJ, Solid Phase.
SO4.
54.19 0 NH^Oi
70.1 0 NHiNOb
84.03
0 NH4NQ,
49.12 6
67.63 2.38
81.38
2.41
45-99 9 -53 NH4N0i+i.3
66.93 346 NH|N0i+ij
81.01
2.45 NU4NQ,+i.3
31.61 19.5 1.3
63.84 4.96 1.3
80.25
2.68 1.3
30.87 20.43 x.3+i.a
58.06 8.22 X.3+X.2
76.01
3.96
31.04 20.4 x.a
52.75 11.42 i.a
73.48
5.14 x.3+i.a
29.81 21.33 "
49.80 13.27 "+(NH|),S04
71 58
5.82 1.3
29.58 41.64 x.a+(NH|)iS04
37.20 19.48 (NU4)tS04
70.15
6.71 x.a+(NIL),S04
5.61 37.89 (NH|),S0»
19.91 28.83
IX. 10
40.81 (NH«)«S04
0 41.4
".05 34.7
0 44.1
0
47.81
1.3 - (NH4)iS04.3NH,NO,. 1.2 - (NH4)2S04.2NH4NO,.
Freezing-point lowering data for mixtures of anunonium nitrate and lead
nitrate are given by Bogitch (1915).
Solubility of Ammonium Nitrate in Nitric Acid.
(GroBchu£F — Ber.37* X488t '04.)
Detenninations by the " Synthetic Method," see Note, page 16.
8
29.5m.pt. 38.8
27.5 44-6
23s 49.4
17.5 54.0
16. 5 54.3
4«o 45-8
Gms. Mds.
NH4NO1 NH4NOS Solid
per zoo per xoo Phase.
Gms. Sol. Mols.HNOa.
21. 1 21. 1 NH4N0s.aHN0s
28.7 31.6 " •
50.0 ••
63.4 - »
76.8
92.4 II
66:7 NH4N(^.HNOj,
Gms. Mols.
NH«NOt NH«NOa Solid
cr xoo Dcr too Phase.
I. Mob. HNOa.
(^.Sol.
a« solution in HNOa,
II. o 51.7 84.3
12.0 54.7 95-1
II. 5 57.6 108.0
II. 5 54.0 92.4
17.0 54-7 95.1
27.0 56.2 lOI.O
49.0 60.4 120.0
79.0 68.1 168.0
b - solution in NH,NO
NE^KOsilNOb
*' lafafl.
h
NHiNOs Ubil.
57
AMMONIUM NITRATE
Sqlubilitt of Ammonium Tri-Nitratb in Water.
(Gxcscfanff.)
r.
Gms. NH|NOk Cms. HNOk Mols. NHtNOk* Mols. NH«NOk
Br xoo total
8
2.S
■ 3
8-5
195
«S
39.5 m. pt.
Solution.
34-2
34-8
per xoo Cms. per xoo Gms. per 100 Mols.
Solution. H|0.
53-9 64.3
54.8
55.8
56.9
58.9
60
61.2
35 4
36.6
37.4
38.1
38 8
75.1
90
"3
225
450
00
Mols. Solution.
22
23.1
24.3
25.7
29
31
33
Solid Phase.
NH4NO8.2HNO1
or NHiNCVaHNOt.
Solubility ov Mixtures of Ammonium Nitrate and Silver Nitrate in
Water at Various Temperatures.
(Schxeinemakexs and deBaat, xgio.)
Gmi.per
xoo Gms.
Gms. per
100 Gms.
Sol.
Solid Phase.
f.
Sol. Solid Phase.
AgNOb. NH«N0^
AgNQ,.
NH«NQ,:
7.3 47.1
0
Ice+xb. AgNOk
109 6
67.9
32.1 D+rb.AgNQi
10.7 44.52
8.43
((
0
22.13
44.87 D+rbJra^NOi
14.9 42
16.8 1
[ce+D+xb. AgNOk
18
27.07
49.22
14.8 39.51
18.79
" +D
30
29.76
52.50
18.7 15.99
17.4 0
0 50.36
18 55 36
30 58.89
37-3
41.2
19-59
22.06
23.42
« +D-Wxb.NH4NQi
" +xb.NH|NOi'
D+xb.AgNOi
II
±32
40
55
85.4
• ■ •
32.68
36.6
• « •
( D+cb. N^70k+
••• \ «+xii.NH4NOb
52.22 D-hiib.NH«NOi
52.38
iD+rb.NH4N0k+
• • • \ rbd.NH,NOi
55 63.32
26.12
If
101.5.
47.5
52.5 D+rbd.NH,NOi
D = N
H4Na.
AgNOi. rb. =
rhombic.
rbd
. a rhombohedric.
Solubilitt of Ammonium Nitrate in Aqueous Solutions of Silver
Nitrate and Vice Versa at 30".
(Schrdnemakexs and deBaat, xgio.)
GoLper 100 Gms.
Gms. per
xoo Gms.
Sat.SoL
Solid Phase.
Sol.
Solid Phase.
AsNQ^
nh«no^
AgNO..
NH4NQ;
0
70.1
NH«NOs
45 85
34.47
D
12.51
6359
u
52.45
28.86
ii
21.31
58.64
tt
57-93
24-33
11
27 -75
54.12
tl
58.88
23.42
D+AgNO,
29.76
52.5
NH4N0,+D
63.27
15.62
AgNQ,
35.62
45.44
D
69.08
6.59
it
41.09
39.60
ii
73
0
it
D « NH4NO,.AgN08.
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. NHiNOs at room temp, with
decomp. (Welsh and BroderBon, 19x5.)
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 % AgNO«. Results for NH^NOs + TlNOs are given by Boks (1902).
AMMONIUM NITRATE 58
Reciprocal Solubility of AimoNiuif Nitrate and Sodium Nitrate in
Water at o**, 15** and 30".
(Fedotieff and Koltunoff, 19x4.)
Sp. Gr. Sat. Gms. per lop Gma. E^.
v^.
Sol.
' NH«N0,.
NaNCV
• .
Sol.
NH«NQm
NaNOk.
0
I -354
0
73-33
IS
1.429
I5S-3
75-38
0
1.407
loss
66
IS
1. 40s
156.1
60.76
0
1.264
118. 4
0
IS
1.364
159
36.50
IS
I -375
0
83.9
IS
I -350
160
27.79
IS
1.386
24.03
81.21
IS
I 330
162.3
17 63
IS
1.392
42.81
79-34
IS
1.298
167.4
0
IS
1. 401
64.6
78.06
30
1. 401
0
96.12
15
1. 417
IIO.9
7S.8I
30
1.450
220.8
88.31
IS
1.428
IS2
7S-3S
30
1.329
232.6
0
Solubility of Ammonium Nitrate in Aqueous Ethyl Alcohol.
(Fleckensteb — Physik. Z., 6, 4x9, '05.)
Grams of NH«NQ| Dissolved per xoo Grams Aq. Alcohol of (Wt. %):
. .
100%.
86.77%.
76.x 3%.
51.65%.
a5.8x%.
0%,
20
2-5
II
''S
70
140
195
30
4
14
32
90
165
230
40
S
18
43
•"5
196
277
50
6
24
55
144
244
36s
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 NHiNOa at 14^ and 3.8
grams at 20.5*.
100 grams absolute methyl alcohol dissolve 14.6 grams NH4NOS at 14^, 16.3
grams at 18.5^ and 17.1 grams at 20.5^
(Schiff and Monsacchi — Z. physik. Chem., az, 377, '96; at 20.5* de Bniyn — Ibid., zo, 783, '92.)
Solubility op Ammonium Nitrate in Aqueous Ethyl and Methyl
Alcohols and in a Mixture of the Two at 30^.
(Srhrrinfmakerg, 1908-09.)
Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol.
H«0.
CtH^H.
NHiNOk.
HiQ.
0
96.4
3.6
0
5
89.6
6.5
S
10
80.4
10.7
10
IS
68.6
17
IS
20
535
26.8
20
25
32.5
44.8
25
29.9
0
70.1
29.9
CH^H. NH4NO1. H^. +c,B$6h. NH4NO.
833 16.7 3.4 84.9 II. 7
74.8 21.3 5 82.9 12,3
63.8 27.1 10 74.6 16.4
50.7 35 15 63.5 24
35.2 46.3 20 48.2 35.1
19.8 59 25 22.4 54
o 70.1 29.9 o 70.1
• Weight per cent CHaOH - 517. CjHftOH - 48.3.
Additional determinations of the solubility of ammonium nitrate in aqueous
ethyl alcohol solutions at o**, 30** and 70° are given by deWaal (19 10). At cer-
tain concentrations at 67.5** the solutions separate into two layers.
59
AMMONIUM NITRATE
AMMONIUM Magnesium NITaATE 2NH4NO|.Mg(NOi}2.
100 parts water dissolve lo parts salt at 12.5^. (Foucroy.)
AMMONIUM Manganic MOLYBDATE 5(NH4)2Mo04.Mn2(Mo207)i.i2H,0.
100 parts water dissolve 0.98 part salt at 17^. (Struve— j. pr. Chem., 61; 460, '54)
AMMONIUM OLEATE CnHnCOONHi.
SOLUBILrTY IN SEVERAL SOLVENTS.
(Fslciola, 19x0.)
SolvenL unU' Min«v.vAjnxi4 aiaaoivca
per zoo cc. soiveni:
Absolute Alcohol 31 at 0** 59 at 10**
75 per cent Alcohol ... 8.2 at 20**
I part Alcohol + 2 parts Ether ... 9 .45 at 15**
Acetone ... 4.7 at 15**
100 at 50*'
10.86 at 30**
16.9 at 20**
• • •
AMMONIUM OXALATE (COONH4)t.HsO.
Solubility in Water.
(Av. curve from results ot Engd, z888; Foote and Andrew, 1905; Woudstra, 191 3; Colani, 19x6.)
* • xoo
is. (COONHJi per
Gms. Sat. Solution.
V.
Gms. (COONHJi per
too Gms. Sat. Solution.
0
2.1
25
4.8
10
3
30
S.6
IS
3S .
40
7-4
20
4.2
50
9-3
Solxjbiliti
' IN Aqueous Solutions of
' Oxalic Acid
•
(Woudstra,
191 2.)
Results at 30**. (Interpolated
from Original.)
Results at 45*
•
Qms. per 100
Cms. Sat. Sd.
SaKd PfMJv
Gms. per xoo Gms. Sat. Sol.
Solid Phue.
(COONH4),.
(C00H),1
^UUU X UbSC.
(COONH4),.
(COOH),.
0.14
12.36
A
0.22
21.22
A
0.28
12.78
A+T
0.31
21.31
ti
0.30
12
T
0.53
20.54'
A+T
0.39
10
«
0.56
21.23
T
0.47
8
((
0.61
20.55
0.52
7
ti
0.54
20.92
0.6S
6
ti
0.79
16.44
I
S
U
1.23
12.88
2
396
u
7.16
7.98
3
3-6i
ii
3-54
5 83
4
360
a
5 65
567
5
3.81
u
6.72
5-95
S.9«
4.21
T+A. 0.
8.74
6.53
T+A. 0.
7
3 63
A.O.
8.93
6.27
A.O.
8.19
3 36
A. O.+N. 0.
9.04
6.14
tt
7
2.32
N.O.
12.38
5 A. O.+N. 0.
6
1.02
It
8.31
3 04
N.O.
S-53
0.22
it
959
1-45
«
A. = Oxalic Add (COOH),.H,0.
A. O. = Acid Ammonium Oxalate (COO)2HNH4.H20.
T = Ammonium tetroxalate (COOH),(COO)aHNH4.2H20.
N. O. = Neutral Ammonium Oxalate (COONH4)2.H«0.
Additional data for this system at 25^ are given by Walden (1905), and at o^
by Engel (1888).
AMMONIUM OXALATE 60
Solubility in Water op Mixtures of Ammonium Oxalate and:
Other Oxalates at 25^. Other Ammonium Salts.
(Foote and Andrew, 1905.) (Colani, 19x6.)
Cms. per xoo Cms. Sat. Solution. m Gms. per xoo Gnu. Sat. SolatioD.
/ * X ^' i -* ^
2.79 (C00NH4)^Hi0 +25.96 (COOK) AO 15 0.I4 (C00NH4)t + 26.35 NH4a
4.8 " +S-7S (coou). so 0.67 - +32.55 "
5^45 " +o.59(cxx))tMg2HdO i8 o.ii - +42.43 (NH4),S04
6.19 " +1.45 (COO), Zn.aH,0 50 O.65 - +45. 92
5.06 " +0 . 28 (CXX)), Cd.3H,0 19 0.085 " +62.26 NH4NOi
50 o.zS " +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®.
(Jfunes, Whittemore and Holden, 19x4.) '
The mixtures were constantly agitated for periods varying from many weeks
to several months.
Gms. per xoo
(NH4),C,04.
Gms. H,0.
Th(C04)|.
SoUd Phase.
Gms. per xoo
(NH.),C,04.
Gms. H,0.
Th(C,Oi)i.
Solid Phase.
5-25
0
(NH4),Q04
29.47
39 10
2*1.7+2.1.2
6.04
1-54
23 04
29.87
2.1.2
7.78
4. SI
16.84
21.18
10.37
8.87
13 27
15.96
15-46
16.89
8.13
913
21.47
26.37
5-36
5-63
28.18
36.54
"+2.1.7
1.70
1.42
2.1.7 = 2Th(C,04)2.(NH4)tC,04.7H,0; 2.1.2 = 2Th(a04),.(NH4),Crf)4.2H20.
100 gms. 95% formic acid dissolve 6.2 gms. (NH4)tCs04 at 21°. (Aschan. 19x3.)
100 cc. anhydrous hydrazine dissolve 44 gms. (NH4)tC204 at room temp,
with evolution of ammonia. (Welsh and BrodervMi, 1915.)
AMMONIUM PALMTTATE CieHsiOsNH4.
Solubility in Several Solvents.
(Faldola, x9xo.)
Gms.
CuHaiO,NH« 1
per xoo CO. of:
r.
Absolute
AlcohoL
75% Alcohol.
50% Alcohol.
Mixture of x Pt.
Alcohol + 3 Paits
Ether.
0
o-S
• • ■
...
• • •
...
10
0.7
1.78
...
0.37 (13°)
0.2 (13»)
20
1-4
4.33
5-33
0.29
a • •
30
...
tl.02
...
• a •
• • •
40
4.5
14.84
6.69
• • •
• • •
so
II
...
...
...
• • •
AMMONIUM PHOSPHATES (NH4)jP04, (NH4),HP04, and NH4H,P04.
100 gms. H2O dissolve 131 gms. (NH4)tHP04 at 15®, iu sat. sol. =» 1.343.
(Greenish and Smith, X901.)
Data for the solubility of mono ammonium phosphate in anhydrous and in
aqueous ortho phosphoric acid, determined by the ^nthetic method, are given
by Parravano and Mieli, 1908.
61 AMMONIUM PHOSPHATES
SoLUBiuTT OP Ammonium Phospbatbs in Aqueous Solutions of Ortho
Phosphoric Acm at 25^.
(Parker, 1914.)
Cms. per loo Gnu.
Solid Phase. Sat. Solution. Solid Phaae.
Gncper
looGms.
SaL Solution.
BJPO^
NH..
4.1
22.6
4-4
18.4
10
131
20
7
30
7-7
34.4
10
40
10.2
48.2
II. 6
H,P04.
NH,.
(NH,)J>04.3H^
40
9 *NH4H2P04
((
30
5-4
it
20.6
4 " .
cc
30
3.8
iC
40
4 "
CNH4)aP04.3H20+ (NH4)2HP04
SO
4.2 "
(NH4)2HP04
60.6
4-4 "
(NH0»HPO4+NH4H2PO4
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 (19 10). The
agreement is satisfactory except for the (NHOsPOi-sH^O end of the curve, for which
much lower values for the NHs component are given by D'Ans and Schreiner.
AMMONIUM Magnesium PHOSPHATE NH4MgP04.6HsO and iHsO.
Solubility in Water and Salt Solutions,
(Bube, 1910.)
The solutions were saturated in jr- 16 liter flasks. The stirrer was introduced
through a mercury sealed, connection, in order to prevent loss of moisture or
anunonia during the long periods required for saturation. Great care was ex-
eidaed to eliminate errors of manipulation. Large volumes of the saturated
aolutbns 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.
Solvent. f. ^^!P' Cms, per too Gma. Sat. Sol Solid Phaae.
**"''™*- •• Saturation. Mg. PA- NH,. ^« *-"*«•
Witer 25^ 69hrs. 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 Mooohydrate
taNHiCI 25 20 days 0.3129 0.3057 ... Mixed hydrates
-:«NH4Cl+i«NH< 25.2 16 hrs.* 0.0249 0.02025 ... Mooohydrate
3-*
0.3 MoL MgClt per liter H/> 25 27 days ... 0.0206 ... Mixed Hydrates
oj " " " " 25.2 16 hrs.* ... 0.0512 ... MoDohydrate
^MoL (NH«)tHP04 per liter H^ 24.25 ... * O.1229 "
Solubility of Ammonium Magnesium Phosphate in Several Solvents.
(Wenger, 1911.)
Gma. NHiMgPOi per 100 Gms. Solvent in:
f.
Water.
]^^
x^
Mixture of i Pt.
Nl^dl?4
NHsper 100.
Aq. 10%
Nfl4Cl+4
NHa per zoo.
0
0.023
O.IIO
0.060
0.0087
• . •
• • •
20
0.052
0.046
0.105
0.0098
0
.0165
0
.0541
30
• ■ •
0.054
0.II3
• • •
■
1 • •
1 . .
40
0.036
0.064
0.071
0.0136
B • •
t . .
SO
0.030
0.072
0.093
0.0153
B • •
• . .
60
0.040
0.085
0.173
0.0174
0.
0274
0.
0731
70
0.016
0.083
0.124
0.0178
1 • •
1 • •
8a
0.019
O.IOI
0.I9I
0.014s
> • •
) • •
AlOf ONIUH PHOSPHATES 63
AlOfONIUM Manganese PHOSPHATE NH4MnPO«.7HA
Solubility in Several Solvents.
(Wenger, 19x1.)
Gms. NHiMnPOi per xoo Gms. Solvent in:
r
w.».* Ag. s% Aq. s% Mixture of x Pt. NIL
^^^' NH^NC^ NHfcl. (d-o.d6)+4 parte lio.
o ... 0.021 0.002 0.0116
20 o 0.020 0.025 0.0122
30 ... 0.023 0.034
40 O 0.021 0.039 O.OI18
SO ... 0.023 0-035 0.0132
60 o 0.027 0.038 0.0194
70 0.005 0.028 0.041 O.OI9I
80 0.007 0.033 0.045 0.0197
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)HPQ|.
xoo grams water dissolve 171 grams (NH4H)HP0| at o% 190 grams at 14.5**
and 260 grams at 31^. (Amat.. 1887.)
AMMONIUM Hypo PHOSPHITE NH4HtPOs.
100 CC. HsO dissolve 83 gms. NH4H2PO1 at room temp. (Squire and Caines, 1905.)
AMMONIUM PERMANGANATE NH4MnO«.
100 parts water dissolve approximately 8 parts of NH4Mn04 at 15^. (Aschoff.)
AMMONIUM PICRATE CeH3(NO,),ONH4.
100 CC. HtO dissolve i.i gm. Am. picrate at room temp. (Squire and C^unes, 1905.)
100 cc. 90% alcohol dissolve. 1.2 gm. Am. picrate at room temp.
(Squire and (Raines, xgos.)
AMMONIUM Fluo SIUCATE (NH4)sSiF«.
100 parts water dissolve 18.5 parts (NH4)tSiF6 at 17.5,° Sp. Gr. 1.096.
(Stolba. X877.)
AMMONIUM SALICYLATE CeH4.0H.COONH4.
SOLUBILITT IN AqUEOUS AlCOHOL SOLUTIONS AT 2^,
(Seidell, 1909* x9zo.)
per 100 Gms. ^£:,L?' OHCOONH« per per 100 Gms. ^Ev^i (XX)NIL perioo
Solvent. Sat,bol. xoo Gms. Sat. Sol. Sat. Sol. J>at. bol. Gms. Sat. SoL
o 1. 148 50.8 70 1. 015 42
20 1. 122 50.3 80 0-979 38
40 1.088 48.3 90 0.936 31.6
50 1.067 46.7 95 0.907 27.8
60 1.042 44.7 100 0.875 22.3
AMMONIUM SELBNATE (NH4}t Se04
100 gms. H«0 dissolve 1.22 gms. (NH4)s Se04 at I2^ (Tuttoa, 1907)
63
AMMONIUM STEA&ATE
AMMOHIUM STBASATE CuHjtOsNH4.
Solubility in Several Solvents.
(Faldola, 19x0.)
Gms. CigHtfOjNHi per zoo cc. of:
r.
o
10
20
30
40
SO
Absolute Alo^L 75% AlooboL 50% AlcohoL
w» X * a • • • •
0.3 0.56
0.9 1.83
1.8 s
0.25
1. 16
3-21
Ether.
O.I
Acetone.
0.08 (i3«)
5 5
AMMOHIUM
SULFATE (NHOsSO^.
Solubility in Water.
(Mulder.)
Gnun» (NH«)iSO^ per 100 GramaL
Grams (NH«)sS04 per xoo Gnmi.
O
5
10
IS
20
as
Water.
70.6
71.8
73 o
74.2
75-4
76.7
Solutioa.
41.4
41.8
42.2
42.6
43 o
43-4
30
40
60
80
100
108.9
Water.
78.0
81.0
88.0
95-3
107 S
Solutioa.
43-8
44.8
46.8
48.8
SO 8
51 -8
Sp. Gr. of saturated solution at 15^ — i 248; at 19^ — 1.241
Eutectic point, Ice + (NH4)iS04 — — 19.05"* and 38.4 gms. (NH^jSOi per 100
gms. sat. solution.
Solubility in Aqueous Ammonia Solutions at 25^.
(D'Ans and Scfareiner, 1910.)
Mob. per 1000 Gms. Sat. SoL
Gms. p>er 1000 Gms. Sat. Sol.
(NH,).
(NHJ,sa4.
0
3.28
1.02
2.60
I -95
2.13
3-44
1-59
S'Z5
1. 16
713
0.78
9-47
0
(NHj).
(NH0»SO;.
0
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 Coffer
Sulfate at 30*' and Vice Versa. •
' (Schreineniakers, 19x0.)
Gma. per loo Gms. Sat.
Scrfutioa.
44
38.32
29.27
17.53
9-33
CUSO4.
o
0.77
1.57
4.05
11.03
Solid Phase.
(NH4)2S04
(NH4)jS04+i.i.6
1. 1.6
a
Gms. per xoo Gms. Sat.
Solution. Solid Phase.
(NHOsSOf. CUSO4.
8.19 13.65
6.98 16.77
5.79 20.53 I.I.6+CUSO4.5H2O
2 . 45 20 . 19 CUSO4.5HSO
20.32
1. 1.6
«
o
* * Solubility of x.x.6 in water.
I.I.6 =» CuS04(NH4)iS04.6H,0.
Several additional determinations for the above system at 19^ are given by
RfidoifF (1873), and by SchifiF (1859}.
AMMONIUM SULFATE
64
Solubility of Ammonium Sulfate in Aqueous Solutions of Ferrous
Sulfate at 30° and Vice Versa.
(Schreinemakers, 1910 &.)
Cms. per 100 Cms. Sat.
Solution.
Solid Phase.
(NH4)2S04
(NH)S0+i.i.6
1. 1.6
it
Gms. per xoo Cms. Sat.
Solution.
Solid Phase.
(NHJjSO^. FeSO^:
44.27 0
43.88 0.79
34.24 1.72
19.64 5.70
16.29 7. 95
(NH4),S04. FeSO*.
8.90 17.64
6.44 23.59
5.91 25.24 I
5.24 25.24
0 24.90
1. 1.6
((
.i.6+FeS04.7HtO
FeS04.7H20
(C
11.45 13 13
II
I.I.6 = (NH4)jS04.FeS04.6HaO.
Data for the quaternary system (NH4)2SO|^ + FeS04 + LiiS04 + HjO at 30*
are^ also given.
Solubility of Ammonium Sulfate in Aqueous Solutions of Lithium
Sulfate and Vice Versa.
(Schreinemakers, Cocheret, Filippo and deWaal, 1905, 1907.)
•
Results at 30®.
Results at so*".
Gms. per 100
Gms. Sat.
Cms. per loo
Gms. Sat.
Solution.
Solid Phase.
Solution.
Solid Phase.
{NHJjSO*.
Li^SOr
(NHOiSO,.
Li^4.
44.1
0
(NHOjSO^
45-7
0
(NH4)«S04
40.8
3
43
05
5.86
(Nti4)sS04+NH«LiS04
39-5
6.6
(NHi),S04+NH.LiS04
19.
65
16.3s
NH4LiS04
30
10
NH.LiS04
13
90
21.20
«
21.6
IS
«
13-
97
21.23
NH4TJS04+Li,S04.H,0
^15
20
it
II.
45
21.75
Li^4.H|0
12. s
21.9
NH«LiS04+Li|S04.H^
9
63
22.79
H
8.9
23
LitS04.H^
8
58
23.09
fl
•
0
251
<i
7
56
22.86
M
•
0
243
If
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, alcohol
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 RfldorflF (1873) to contain 37.97 gms. (NH4)tS04 + 39.3 gms.
K2SO4 per 100 gms. sat. solution.
Solubility of Ammonium Sulfate in Aqueous Scm^utions of Sulfuric
Acid at 30".
(Van Dorp, 19x0 and 19x1.)
Gms. per 100 Gms. Sat.
Solid Phase.
Gms. per xoo Gms. Sat.
Solution.
(frao^soT
44.3
43-6
44.1
42.9
41
40.8
43
4S-5
42.3
HtS04.
O
10
13.2
IS
20
25
30
33.8
35
(NH4)2S04
(NH4)2S04+3.i
Solution.
(NH4),S04. hJsqT
3-1
32.8
26.1
20.9
17.6
17.8
20
30
37
3.i+(NH4)HS04
(NH4)HS04
3.1 =3[(NH4),S04].H,SO.
40
45
50
55
60
61.7
62.9
62.2
SoUd Phase.
(NH4)HSO
(t
((
tc
u
CI
(C
ct
65
AMMONIXTM SULFATE
Data for the solubility of ammonium sulfate in aqueous solutions of sulfuric
add of concentration extending to lo gm. mols. per liter, are given by D'Ans
(1909 and 1913)-
Data for the solubility of ammonium and lithium sulfates in concentrated
suuuric acid containing traces of water, at 30^ are given by Van Dorp (19 13-14).
SoLUBiLiry OF Ammonium Sulfate in Aqueous Solution of Ethyl
Alcohol at 30® and at 50'.
(Results at 30*, Wibaut, 1909; at 50% Schreinemaken 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 Solutioii.
Gms. per 100 Gms. Sat. Solution.
(NHJjSO,.
CADH.
Bfi.
(NHJ,SO«.
C|H,OH.
H^.
2.2
56.6
41.2
371
5-8
57-1
2.6
S4S
42.9
35-7
6.3
S8
3-4
52 -3
44.3
33-8
7-4
58.8
13-2
318
ss-
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)sS04 per 100 gms. sat. solution, At 90.4% alcohol no (NH4)sS04
is dissolved.
Results at 50^
Gms. per zoo Gms. Saturated Solution.
(NHJtSO*.
CiHiOH.
H,0.
43.02
2.32
54.66
41. 1
4.1
S4.8
1.2
64. s
34.3
0.2
7SS
24.3
Between the concentrations 4.1 and 64.5% CsHtOH 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 zoo Gms. Sat Solution.
Gms. ]
per zoo Gms. Sat. Solution.
(NHJtSO..
QH^H.
HiO.^
(NHJtSO*.
C|H,OH.
HjO.'
1.2
64s
34.3
41. 1
41
54.
.8
1.6
60
38.4
36.8
6
57.
.2
3-8
SO
46.2
30.8
9
60.
.3
7.4
40
S2.6
26.6
12
61.
■4
10
34.4
SS'^
23,6
15
61
•4
Two determinations at o^ by deWaal (1910) gave 30 gms. (NH4)2S04 per 100
gms. sat. solution in 9.41% alcohol and 0.14 gm. (NH4)sS04 in 73.03% alcohol.
Between these concentrations of alcohol two liquid layers are formed.
100 gms. 95% formic add dissolve 25.4 gms. (NH4)tS04 at 16.5°.
(Aschao, 19x3.)
AMMONIXTM SULFATE 66
Solubility of Ammonium Sulfate in Aqueous Ethyl Alcohol Solutions.
(CarUinued,)
CTnnbt and Neuberg — Z bbysik. Chcin. i> 510, '87; BodUmJer — Ihid, 7t3xS» '91; Sdudnemaker —
Ibid. 23, 657. '97 ; de Brujn— Ibid.S^, 68, '00; linebarger — Am. Cn. J. Z4f 580^ '9>«)
Upper Layer Remits.
Lower Layer Results.
Grams per xoo Gms. Solu-
tion at io'-4o**.
Gms. CiILOH
per 100 Gms.
Solution.
Gms. (NH4)sS04 per
SolutioQ at:
100 g.
C^QiOH.
(NH«)aS04.
'6.f.
IS**.
33^
100
00
0
42.0
42.6
44
80
01
2-5
39 0
40.2
?
70
03
50
36.2
37-2
?
60
14
7-5
33-2
34-5
42
SO
3-2
10. 0
30 0
31.0
35
4S
4.8
"5
27.2
28.0
?
40
6.6
15.0
24.6
25.2
?
35
9.2
175
22.0
22.4
?
30
12.2
20.0
20.0
20.0
?
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 takien 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®.
(Uoebarser— Am. Ch. J. 14, 380, '93.)
Gms per xoo Gms. Gms. per xoo Gms.
Solutian. Soli
lution.
C^tOH. (NH4)sS04. QHtOH. (NH«)sSQ«.
70 0.4 40 3.2
60 i.o 30 4.8
50 2.0 20 6.7
67 AMMONIUM Cadmium SULFATE
AMMONIUM Cadmium SULFATE (NH4)tCd(SO«)s6HsO.
100 cc. HiO dissolve 72.3 gms. (NHOtCdCSOOi at 25^ (Locke. 1901.)
AMMONIUM Chromium SULFATE (Alum) (NH4)tCrs(S04)4.24HsO.
100 cc. H^ dissolve 10.78 gms. anhydrous or 21.21 gms. hydrated salt at 25**.
(Locke, X90Z.)
AMMONIUM Cobalt SULFATE (NH4)tCo(SO«),.6H^.
Solubility in Water.
»«M<^ ^
Ck J. 27. 459i
'ox.)
ji j«*t •■• "J f
Gnu. (NH«)sCo(S04>s
Gms. (NH4)sCo(S04>s
*•.
per xoo
Gms.
t*.
per
100 Gms.
Water.
Solutioii.
Water.
Solutioo.'
0
6.0
5-7
40
22.0
18.0
10
95
8.7
so
27.0
21.3
20
13 0
"5
60
33 S
251
25
14.72
12.8
70
40.0
28.6
30
17.0
US
80
49 0
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 cvirve.
AMMONIUM Indium SULFATE (NH«)sInt(SO«)4.24HsO.
100 gms. HjO dissolve 200 gms. salt at 16° and 400 gms. at 30^. (ROasler, z873*)
AMMONIUM Iron SULFATE (Alum) (NH4)iF^(SO«)4.24HsO
100 cc. HsO dissolve ^
25^ Sp. gr. of saturated £
100 cc. HsO dissolve 44.15 ^ms. anhydrous or 124.40 gms. hydrated salt at
solution at 15 = 1.203. (Locke, igoi.)
AMMONIUM Iron SULFATE (ferrous) (NH4)sFe(SO«)s.6HsO.
Solubility in Water.
(Tobler; at 35^ Locke — Am. Cb. J. 2KK, 459, 'ox.)
t<».
G. (KH«)3Fe(S04)s
per xoo g. HsO.
f.
G. (NH4)3Fe(S04)a
per xoo g. H2O.
*•.
G. (NHt)iFe(SO,)i
per 100 g. BiO.
0
12. 5
25
250 (T)
SO
40
IS
20.0
2S
40
3Si(L)
33 0
70
s«
AMMONIUM Lead SULFATE (NH«),S04.PbS04.
Solubility in Water.
(Barre, 1909.)
f . Gms. (NH4).SO. per xoo Gms. ^^ pj^
Sat. SolutioQ. Water.
20 12.17 13.86 (NH4)2S04.PbS04
50 16. IS 19-25
75 1952 24.31
xoo 22.74 29.42
u
it
it
AMMONIUM Lithium SULFATE 68
AMMONIUM Lithium SULFATE NH«LiS04.
SoLUBiuTY IN Water.
(SchidDemaken, Cocheret, Filippo and deWaal, 1905, 1907.;
G11W.NILUSO4
per 100 Gins.
Gnu.NHJiSOt
per 100 Gnu.
r.
SoUd Phase.
f.
SdBiPhtM.
Sat. Sol.
m
Sat. Sol.
0
0
Ice
— 10
35-25
NHJ,iS04
- S
14
((
fio
35-58
tt
— 10
23s
it
30
^K.Sj
tt
-IS
29.7
it
SO
36
tt
— 20.6Eutec.
3S.IS
Ice+NHtLiS04
70
36.18
tt
u
M
AMMONIUM Magnesium SULFATE (NH«),Mg(SO«)t.
Solubility of Ammonium Magnesium Sulfate in Water.
(Porleua, 1914.)
^ Gnu. per xoo Gms. _ ... _. ^ Gms. per xoo Gms. „ ,.^ ^,
r. c > cIi ' ur > — Solid PhaK. r. c , cT, " u; , > SoUdPhaie.
Sat. Sol. Water. Sat. Sol. Water.
—0.34 1. 01 1.02 Ice 20 15.23 17.96 (NHJtMgCSOJt
—0.80 2.98 3.07 " 2$ 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 .34 EuteC Ice+(NH«),Mg(SO0t 60 26. 02 35 . 17 "
O 10.58 11.83 (NHi)MgS04 80 32.58 48.32
10 12.75 14.61 " 100 39.66 65.72 *
AMMONIUM Manganese SULFATE (NH4)sMn(S04)i.6HsO.
100 cc. water dissolve 37.2 gms. (NHOsMnCSOi)! at 25^. (Locke, 1901.)
AMMONIUM Nickel SULFATE (NH«),Ni(S04)i.6H,0.
Solubility in Water.
(Awra«e curve from Tobler, Locke, at 95^.)
G. (NH4)sNi(S04)a G. (NH«)tNi(SQ«)i
per loo Gms. . ^•, per 100 Gms.
Water.
Solution.
Water.
Solutiaa:
0
I.O
0.99
40
12.0
10.72
10
40
3-85
50
14.5
12.96
20
6-5
6.10
60
17.0
14.53
25
7-57
7.04
70
20. 0
16.66
30
9.0
8-45
AMMONIUM Sodium SULFATE NH4NaSO«.2HsO.
100 gms. water dissolve 46.6 gms. NH4.NaSO4.2HaO at 15* Sp. Gr., of Sol.
1.1749.
AMMONIUM Strontium SULFATE (NH4}tS04.SrS04.
Solubility in Water.
(Barre, 1909.)
*• Gms. (NH4)>Sp4 per 100 Gms.
&t. Solution. Water.
SO S43-99 78.54 (NH4)2S04.SrS04+SrS04
75 45.40 83.15
100 46.27 66.2
69 AMMONIXTM Vanadium SULFATE
AMMONIUM Vanadium SULTATB (Alum) (NH4)iV,(S04)424HsO.
100 oc HsO dissolve 31.69 gms. anhydrous or 78.50 gms. hydrated salt at 25**.
CLocke.)
AMMONIUM Zinc SULFATE (NH4)iZn(S04)s.6H,0.
Solubility in Water.
(Avenge curve, see Notb» p. 67, Tobler, Locke, at 35*.)
••.
G. (NH«)A<S04)t
per 100 Gms.
Sdutioa.
Water.
0
10
90
6.54
8.67
II. II
7.0
9S
12.5
as
30
12.36
13 -79
14. 1
16.0
t».
G. (NH4)>Zd(S04)i
per TOO Gms.
40
Soltttioa. WatarT
16.66 20
SO
60
70
80
20.0 25
23 I 30
as -9 3S
29.6 42
ato*.
(MarshaU, z89z.|
AMMONIUM PEBSULFATE (NH4)iS,Q8.
100 parts H«0 dissolve 58.2 parts (NH4)iS2C^ at o**.
AMMONIUM Sodium Hydr(%en SULFITE (NH4)NasH(SO,)s4HsO.
100 gms. HsO dissolve 42.3 gms. salt at 12.4° and 48.5^ gms. at 15**.
(Schwincker, 1889.)
AMMONIUM Antimony SULFIDE (Sulfoantimonate) (NH4)iSbS4.4HsO.
Solubility in Water and in Aqueous Alcohol.
(Donk, 1908.)
In Water.
Gms. (NH«)iSbS|
per ICO Gms. Sat. Sd
9.9
20
30.2
41.6
41.6
47-7
54. S
Solid Phase.
Ice
u
It
In Aqueous Alcohol at io*«
Gms. per xoo Gms. Sat. Solution.
Ice+(NH«),SbS4.4lW)
(NH«)iSbS4.4HiO
U
It
CAOH.
(NH4),SbS«.
0
43.2
S-i
3S.9
19. 1
23.1
43.1
8.7
S3'^
4.1
93-3
0
r.
- 1.9
" S
- 8
-13. S
o
+20
30
AMMONIUM /7-Naphthalene Mono SULFONATE CioHi7SO,NH«.
100 cc. of the saturated aqueous solution contain 13.05 gms. of the salt at
25**, and d» = 1.034. OVitt, 1915.)
AMMONIUM Phenanthrene Mono SULFONATES C14H9SO1NH4 (2), (3) and
^'^^' Solubility in Water at 20".
(Sandquist, 1913.)
100 gms. HsO dissolve 0.37 gms. Ci4H»SOiNH4 (2).
100 gms. HsO dissolve 0.26 gms. Ci4H»SOsNH4 (3).
100 gms. HsO dissolve 4.41 gms. C14H9SO1NH4 (10).
AMMONIUM 2.5 di-iodobenzene SX7LF0NATE CeH,IsSO,(NH«).
100 gms. HsO dissolve 4.35 gms. salt at 20*^.
(Boyle, 1909.)
(Fenton, 1898.)
AMMONIUM TARTRATES (NH4)sC«H40«.
100 cc. HsO dissolve 2.83 gms. (NH4)sC4H40«.2HsO at o*.
100 cc. HsO dissolve 5.9 gms. (NH4)8C4H40« at 15° (d - 1.04).
(Greexush and Smith, 1903.)
AMMONIUM Lithium TARTRATES dextro and racemic.
100 gms. sat. sol. in HsO contain 13. 104 ^ms. racemate (NH4)Li(C4H40«).HsO at 20^
100 gms. sat. solution in HsO contain 14.186 gms. dextro (NH4)Li(C4H40i).
i HsO 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).
u
tt
AMMONIUM TmOCYANATB 70
AMMONIUM THIOCYANATB NH4SCN
Solubility in Water. .
(Average curve frcnn results of RQdorff, 1868 and 1873; Wassilijew, 1910: Smits and Kettner, I9xa.)
A. Gms. NH4SCN Q^,;j pu.^ A4I Gms. NH^SCN Solid
•• per 100 Gms. Sat. SoL aoua rnasc. r. per 100 Gms. Sat. Sol. Phase.
— 10 20 Ice o 54.5 NH4SCN
-IS 28. s " +10 59
—20 35-5 " 20 63 "
— 25.2 42 Eutec. Ice+NH4SCN 25 65.5
-10 so NH4SCN 30 67.5
Data for the system ammonium thiocyanate, thiourea and water at 25** are
given by Smits and Kettner (19 12) 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 NH4SCN.4(NH4)iCS is formed.
100 gms. acetonitrile dissolve 7.52 gms. NH«SCN at i8^ (Naumann and Schier. 19x40
Freezing-point curves have been determined for the following mixtures:
Ammonium Thiocyanate + Ammonia. (Bradley and Alexander. 29x3.)
" 4- Potassium Thiocyanate. (Wnesnewaky, 191a.)
" " -h Thiocarbamide (Thiourea). (Renolds and Werner, 1903;
Findlay, 2904; Atkins and Werner, 2912; Smits ajid Kettner, 2922; Wrzesoewaky, 29x3.)
AMMONIUM URATE (Primary) CiH,N«0sNH4.
Solubility of the Lactam Ain> Lactim Forms in Water.
(Gudzeit, 2908-09.)
Gms. of Each per xooo cc. Sat. Solution.
f. / * V
Lactam. Lactim. Mixture of the Two.
18 0.456 0.304 0.414
37 0.817 0.540 0.741
AMMONIUM Meta VANADATE NH4VO1.
Solubility in Water and in Aqueous Ammonium Salt and Ammonium
Hydroxide Solutions.
(Meyer, 2909.)
Gms.
per 2000 cc. in
I Each Solvent.
V.
m
Water.
0.05 n.
NH4CI.
o.i n.
NH^Cl.
0.05 n.
NH4NO,.
0.2 n. 0.0668 n.
NH4NO,. NH,.
0.945 D.
0.588 n.
NHi.
18
4. 35
1.66
0.41
1.67
0.58 5.58
7-97
12.06
25
6.08
2.63
1. 17
2.77
1.23 7.06
8.58
12.66
35
10.77
5-21
2.69
• • .
• ft ■ • • •
• • •
...
45
15-71
8.88
5 40
• . .
• • • « • •
• ••
• • •
55
19.97
II. 18
7.40
• • .
• • • • a •
• • t
• • •
70
30.47
...
f 1 «
...
...
• • • • • •
• • •
• . •
1 .
100 cc. anhydrous hydrazine dissolve 2 gms. ammonium metavanadate at
room temp. (Welsh and Broderson, 2925.)
ABIYaDALIN CsoHsTNO.aH.O.
100 gms. trichlorethylene dissolve 0.029 S™* amygdalin at 15^.
(Wester and Bruins, 2914.)
AMYL AOETATE BUTYBATE, FORMATE, etc.
Solubility in Water and in Aqueous Alcohol at 20**.
[(Bancroft— Phys. Rev. 3. 231, 296, ao5, *9S-*96; Traubc.— Ber. 17, 2304. '84^
200 cc. axJ» 01 i!iSter. 200 oc. tisHJ* ot luaet.
Amyl 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 o . 06 0.85
71
AMn ACSTATE
SoLUBiLiiT IN Aqueous Alcohol at Room Tbmpbraturb.
(Pfeiffer, 1892.)
Solubility of Iso Amyl Acetate Solubility of Amyl Acetate and Amyl
in Aq. Alcohol Mbctiu^s. Formate in Aq. Alcohol Mixttires.
Fte 5 cc. CaEbOH.
ccHjlO.
7
6
5
3 -61
3<ii
2.60
ocJboAm^
acetate.
0.41
0.7
I 31
30
4.0
50
4
tt. C^H^H
in Mixture.
cc. HaO added to cause aeparatioo
of second phane in mixtures of the
. given amounts of alcohd and 3 oc.
portiona c^:
Amyl
Formate.
Amyl'
Acetate.
3
1.80
1.76
9
8.77
9
03
15
17.01
17
•52 •
31
27 06
26
99
27
38-31
37
23
33
50-71
48
41
39
65.21
• 4
1 •
45
85.10
• • •
48
94 20
• «
1 •
AMTL ALCOHOL COlnOH.
Solubility op Amyl Alcohol in Water at 22**.
(Herz — Bcr. 31, 2671, '08.)
100 cc. water dissolve 3.284 cc. amyl alcohol. Sp, Gr. of solu-
tion « 0.9949, Volume — 102.99 cc.
100 cc. amyl alcohol dissolve 2.214 cc. water. Sp. Gr. of solu-
tion = 0.8248, Volume = 101.28 cc.
Sp. Gr. of HaO at 22° « 0.9980; Sp. Gr. of amyl alcohol at 22°= 0.8133.
SoLUBiLmr IN Aqueous Solutions of Ethyl Alcohol.
(Pfeiffer, 1892; Bancroft, 1895-96.)
Mixture of
cx.H/>
Wax
added to*
Mixture of
ccHdO
MJxt
Added to*
C^aOH+CAOH
ureat
CftHuOH+C|H.OH
.ure at
ex. ex.
9.1*.
19.2".
ex. cc.
13.3*.
17. 4*.
3 3
3.21
3-5
3 3
3.36
3.47
3 6
10.3s
10.80
6 3
2.20
2.2s
3 9
18.34
19.10
9 3
2.10
2.15
3 13
27.47
29.15
12 3
3.10
2.10
3 IS
41.25
43.15
IS 3
3.10
3.10
t* JoBt enough ?ntter was added to piodooe fkwidinfM.
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 eth)rl alcohol + 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.
DfSTBIBUnON OF ISQAMYL AlCOHOL BETWEEN WaTER AND COTTON SEED
Oil at 25°.
(Wroth and Reid, 19x6.)
Cms. C^uOH per 100 cc. . ^ .
)aUyer.
H^ Layer.
1.947
0.9153
0.470
2.195
I.II56
0.508
2.273
I . 1050
0.486
3.372
0.9995
0.421
AMTL ALCOHOL 72
S(H.UBILITY OF AllYL ALCOHOL IN WaTBR AND IN AQUEOUS SOLUTIONS OF
Ethyl and Methyl Alcohols. '
m
(F(Niteiii, 19x0.)
In Water. In Aq. Ethyl Alcohol.* In Aq. Methyl AlcohoLt
Gms. CiHuOH per Cms. C|HuOH per Cms. CiHnOH per
100 Gna. ., 100 Gms. ^ loo Gms.
TJO C«HuOH QH^H+HiO C,H„0H " CH,OH+H|0 OHaOH
Layer. Layer. Layer. Layer. Layer. Layet.
0.5 4 ... 4.5 16.2 ... 3.6 II
15.5 2.6 90.7 20 20.8 ... 20 19.3
20 2.6 90.6 40 26.7 ... 38.4 ... 78.4
40 2.1 89.5 60 33 ... 40 31.2 78
60 a 88 67.8 ... 24.4 so 37.1 74.8
80 2.S 86 70 36. s 73-7 60 43.3 71.6
100 3 83.8 80 40.8 70.1 70 52.7 6s
120 3.8 80.8 90 47 64 72 (crit. temp.)
140 5 76 . 4 94 . 2 (crit. temp.)
160 7.3 70
170 9-3 65.1
180 13. s 57-3
187.5 (crit. temp.)
* Of 33.5s per cent C|H|OH. t Of 33 per cent CH^OH.
The ''synthetic method" was used for the preceding determinations. Fer-
mentation amyl alcohol of b. pt. I3I*'-I3I.a* and du.^ =0.814 ^^^^ 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 temarv
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.
ABRL ABmnB CiHu.NHt.
#
The freezing-point curve for mixtures of amyl amine and water is given by
Pickering (1893;.
Iso AMTLAMINE HTDBOCHLORIDE CiHu.NH,.HCl (iso).
100 gms. HsO dissolve 192.2 gms. of the salt at 25^. (Peddle and Tuner. 1913.)
100 gms. CHCU dissolve 5.1 gms. of the salt at 25**.
Data for the distribution of €-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).
■
AMTLENE (Trimethylethylene) (CH,)tC:CHCH,.
RsapROCAL [SoLUBiLiTy IN Aniline; Detbrminations bt Stnthbtic Method.
(Konowalow, 1903.)
t*. Gms. Aniline per zoo Gms. «• Gms. Aniline per zoo Gms.
Amylene Layer. AnUine Layer. ' Amylene Layer. Aniline Layer.
0
19s
81. s
10 28
73
2
19.7
80.5
la 34
68
4
20.5
79-5
13 . 38-5
64.7
6
21.7
78
14 45 ^
59
8
24.2
7S-8
14 . 5 (crit. temp.) 51.6
.'73 AHTUENE
Soi.UBiLmr OF Aicylbnb in LiQum Carbon Dioxidb.
(Bilchner, 1905-^.)
(Determinations made by the synthetic method.)
t*. (crit.) 31 103 201
Gms. C5H10 per loo gms. sat. sol. o 38 100
AMTLENE HTDRATB (CH,},C(OH)CHi.CH,.
"The distribution coefficient of amylene hydrate between olive oil and water
at ocd. temp, is i. (Baum, 1899-)
ANDROMEDOTOXINE CaHuOu.
Sqlubilitt IK Sbveral Solvents at 12^ and at thb Boiling-Points of
THB Solvents.
(Zaayer, 1886.)
*
Gms. CnHuOu per zoo Gms. Sat. Sol. at :
Water
Ethyl alcohol {dn =
Amyl alcohol
Chloroform
Commercial ether
Benzine
^U5 (p Propylanisole) <
0.821)
CHiCHCI
xa*. B. Pt.
2.81 0.87
11.70
1 . 14
0.26 0.26
0.07 0.07
0.004
lUlCeHiOCHi.
Solubility in Aqueous Alcohol at 20"
(Scbimmel and Co., Reports, Oct. 1895, p. 6.)
Vol. per cent alcohol = 20 25 30 40 50
Gm. anethole p>er 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.
(Squize aad Gaines, 1905.)
Freezing-point data for mixtures of anethole and menthol are given by Scheuer
(1910).
ANIUNB CeHsCNHs).
Solubility in Water at 22**.
(Hers, 1898; see also Vaubel, 1895; Aignan and Dugas, 1899.)
Toocc- HsO dissolve 3.481 cc. CeHtCNHi) — Vol. of Sol. = 103.48, Sp. Gr. =
a9986.
100 cc. C«Hi(NHt) dissolve 5.22 cc. HtO — Vol. of Sol. = 104.96, Sp. Gr. =
1.0175.
100 cc sat. aq. sol. contain 3.607 gms. CsHsNHs at 25^. (Reidel. 1906.)
SoLUBiUTy OF Aniline in Water. (Determination by synthetic method.)
(Sidgwidc, Pickford and Wilsden, 29x1.)
Gms. C<H«NHgj)ei<'ioo Gms.
Aq. Layer. Aniline Layer.
120 9.1 14.6
130 II. 2 16.9
140 13. s 19s
ISO 17. 1 24
160 22 32
165 26 . I
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 lOO cc. of mixture, are
Kiven by Koltho£F (1917).
r.
Aq. Layer.
Aniline Layer.
13.8
3 -611
S-isCao")
30
3-7
5-4
so
4.2
6.4
70
5
7-7
90
6.4
9.9
no
8
13
ANIUNB
74
Solubility of Aniline in Aqubous Solutions of Aniline Hydrochloride.
(Sidgwkk, Picklord and Wilsden, 19x1.)
The temperatures at which a second liauid phase separated from homogeneous
mixtures ot known amounts of aniline + HCl + HsO 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 olseparation was taken as that at which
a small gas name seen through the lic^uid 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. HCl (of different
strengths) and aniline were determined. By interpolation from these, the fol-
lowing isothermal curves were obtained.
Isotherm
for 15'.
Isotherm
for 25".
nfi Rich Mixtures.
Amline Rich Mixtures.
ELO Rich
uma. per
Mixtures.
Aniline Rich Mixtures.
Cms. per zoo Cms.
Cms. per
zoo Gms.
zoo Gms.
Gms. per zoo Gms.
Sat.1
Solution.
Sat. Solution. '
Sat. Solution.
Sat Solution.
QH.NH,.
C^HftNH^HCL
HdO. CANH,.HCr.
CHaNHf. <
::;anh,.hci
. Hfi. CANHflJia
3.61S
0
7.276
3 025
3.681
0
14
8.884
3791
I 529
7-231
1.989
4.020
3.02
10.84
6.062
4.144
5.829
S.816
I -195
5.380
11.40
6.949
1. 912
4.940
11.44
5 230
0.340
7.023
15.83
6 .043
0.828
S-99S
16.03
5.006
0.163
11.86
19.02
5.568
0.363
10.44
1935
4.960
0.080
31.35
20.15
53"
0.089
26.80
21.49
4.942
0
59.95
15.55
5.299
0
Isotherm for 40**.
Isotherm for 60^.
3 941
0
15.65
8.752
4.58
0
14.27
5.93
4.187
1.523
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
S.81S
7.069
1.452
567
5.762
7.492
0.4876
6.210
11.30
7.058
0.9669
7.69
II. 14
7-051
0.2284
8.779
^S'55
6.225
0.4052
"53
15.25
7.047
0.1 138
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 80^.
Isotherm for 100**.
5-66
0
12.31
3.387
7.10
0
41.57
"45
S-9S
1-495
9.848
1.350
7.68
1.467
18.16
4.^5
6.26
2.950
8.998
0.5857
8.10
2.891
12.76
1.784
7. II
5.678
8.524
0.2769
9.60
5.522
"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^.
Isotherm for 140"*.
9 30
0
17.94
2.459
13.75
0
29.52
4.043
31.21
9-497
14.45
0
38.75
7.384
21.09
0
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 + HCl + H,0 at o*. 25* and at 35**
are given by Thonus (1913), and for aniline -h HCl by Leopold (1910).
75 AMIUIIS
Solubility or Aniune in Aqueous Salt Solutions at iS\
(Euler — Z. phystk. Chem. 4gb J07, '04.)
Aq.8diitiaa. Gm..S*lt Gm*. C:.H.(NH^ Aq. Gms.Salt Gii».C.HrfNH,)
gM^. wtawMJu. pg^ iijgy^ p^ jQ^ ^^ aolwnt. Solttdon. per liter. perzoog.aolTeBt.
H2O alone o 3.61 i nNaOH 40.06 1.90
o.5f}KCl 37.3 3.15 I nLiCl 42.48 2.80
I nKCI 74.6 2.68 I nCaCls 67.25 3.00
I nNaCl 58.5 2.55
Solubility of Aniline in Aqueous Aniline Hydrochloridk
Solutions at 18°.
(lidow — J. russ. phys. chem. Ges. Z5* 4«>, '83; Ber. i6» M97, "Ea.)
Per cent CaHflNHsHQ Gms. CsN<NHs Ptt cent CsHsNHa.Ha Gdis.CbHsNI^
inSol^rent. per 100 g. Solvent in Solvent. perxoog.SdvcnL
5 3-S 30 39-2
" 5-3 35 so -4
Solubility of Aniline in Aqueous Solutions of Glycerol and
Vice Versa.
(Kolthoff, 19x7.)
(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 Gbceiol in ^^ Aniline dissolved by xoo oc of Aq. Glycerol of Cone, shown at:
Aq. Mixtuie used. ^-^JT ^^7 ^^T "^^ ^
o(= water) 3.25 3.4 5.6 9.9
39 S-^S S'S
$6 7.5 7.6 ... 28 (58% Glycerol)
6s 10 ... ... 38(66% " )
74.3 II-7S i^-^
78 20 20 16
07 7 ... ..■ ..•
Results for the Solubility of Aqueous Glycerol in Aniline.
Per .j^t^t Glycerol in cc. of Aq. Glycerol Mixture dissolved by loo cc. Aniline it:
Aq. Mixtuic nmd. '^ -^ ^ ^T ^
o(= water) 4.6 5 4 5.3
39 ••• 6.4
47 S-2
56 7-9 7.7
74.3* 131 "7
78 17. 1 14.8
IS (S8% Glycerol)
17(66% " )
Distribution of Aniline between Water and Benzene at 25^
(Fanner and Waxth, 1904.)
Gms. CANHs per zoo cc.
/ * N Ratia
Water Layer. C«H^ Layer.
0.013s O.I312 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; 0, m and p nitraniline, chloraniline, bromaniline.
P nitrosmethylaniline, and p nitrosodimethylaniline are given by Farmer and
Warth (1904;.
ANILniE 76
SoLUBiLrry of Aniline, Phenol Mdctures in Water.
(Schrdnemaker — Z. physik. Chem. 39. 584; 30» 460, 'qq.)
MiTture used ■■ a«^ Mols. Aniline Mixture tifled«-<o Mols. Aniline
4- 74 6 Mob. Phenol « +50 Mob. Phenol
Gms. of Mixture per xoo Gms. * * Gnu. 01 Mixture per xoo Cms.
"^Aq. Layer.
A. + P- Layer.
Aq. Layer.
A.+P. Ltrc-
40
S-O
86.0
40
4.0
91 5
60
SS
82. 0
80
5-5
8SS
80
80
77 0
100
80
83 0
100
"S
67 0
120
13 S
73 5
no
19.0
56 s
130
19.0
660
104
(crit temp.)
33
• * •
^3S
23 S
S8o
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] 67i 477t '03.)
Water and Ether. Water and Carbon Tetrachloride.
Comporitioii of Solutions. Gms. CANHain: Composition of Solutions. Gms.CeHiNHtin;
1.2478 so CO. HjO 50 CO. HjO
+ 20CC. Ether 0.1671 1.0807 0.3478 +20CC.CCI4 0.33580.0x3
1.9478 50 cc. Hjp 50 CO. H.O
+SOCC. Ether 0.0835 ^'^^43 1.2478 +5000. CCI4 0.2767 1.971
1.2478 50 cc. HjO 50 cc. HjO
+Z00CC. Ether 0.0594 z.1884 1.2478 + 100 CC.CCI4 0.1845 1.063
Solubility of Aniline in Sulphur.
(Alexejew — Ann. Phyak. Chem. 28, 305, '86)
«• Gbm.CsHsNHs per 100 g. , Gms. CsHBJNHt per 100 f .
S. Layer. Anilin Layer. S. Layer. Anilin Layer.
100 4 75 130 IS S^
no 6 70 13s 17.5 47
X20 to 64 138 (crit temp.) 23 . .
Distribution of Aniline between Water and Toluene at 25*.
(Riedd« 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 * ^m' P^*?** % ?* **^ ^* "^ Gms. CeHgNgi in 100 cc. cl;
ArT» ?irj3*™L Anflfaie : Toluene Mixture after «. _ _ ' . - >.
A. T Mixture. In Mixtures Used. Separation. A :T Layer. Aq. Layer.
1^0 50:50 0.9257 41-5 2U
25:75 0.8928 20.7 1.5
12.5:87.5 0.8737 8.62 0.86
SS'-94-5 08661 3.87 0.45
2*5'*97*5 0.8627 1.68 0.21
14
U
The author also gives data for the distribution of aniline between toluene
and aqueous solutions of K|S04, KBOi, Ba(OH)s, Sr(OH)i and Ca(OH)i.
77
AHnJNE
Solubility Data Dbtekmined bt the Freezing-Point Method (see foot-
note, page i) ARE Given for Mixtures of Aniline (m. pt. —5.5° to —6,8*)
AND Othek Compounds.
Name and M. Pt. of the Other Com-
pound d Each Mixture..
Nitrosodimethyl aniline (85.5^)
Benzene (5.42 )
Nitrosobenzene (^s.s'O
Nitrobenzene (2.8^
0 Dinitrobenzene (116.5**)
« " (91")
P
s Trinitrobenzene (122.2*^
0 Chloronitrobenzene (32 )
« " U3")^
p " (82.5**^
Benzoic add (121.25°)
Chloroform (—63°)
0 Ciescd (30.4°)
m " (4.2°)
P " (33.0
Ethylacctatc (-83.8*)
Hydroquinone
Allyl mustard oil
o Chlorophenol
o Nitiopnenol (46^
Data for Firat Eutectic
w iH Wt. Per Cent.
- 9.2
94.2
-12. 5
77.2
—30 -6
53.4
—10
92.2
- 8
92. 7«
no eutectic
not determined '
-19. S
66.1
—12.6
79.7
-16.3
72.7
• • •
-71
• « •
21.7
-17
78.8^
-30
74.3 •
-15. 5
8S.S'
Authority.
(Kiemann, 1904.)
(Kremann and Bocjaoovics, 1916.)
(Kremann. 1904.)
•I
(Eiemaon and Rodinis, 1906.)
(Kremann. 1904-)
(Kremann and Rodinis, 1906.)
(Kremann« 1904.)
(Kremann, 1907.)
(Kremann and Rodinis, 1906.)
•I
M
(Baskov. 19x3-)
(Tsakalatos and (Svye, z9xa)
(Kremann. 1906.)
u
89
62
(Kremann. 2906: Philip. i9o3>)
(Wroczynski and Guye, 19x0.)
(Kremann and Rodinis. 1906.)
(Kumakov and Kriat. X913.)
(Kumakov and Solover. 19x6.)
«
(96I
P " ("3^)
m Dinitiophend (110.5^
Pyrocateoiol (105°)
Resordnol (110°)
Nitiotoluene (si'3*)
Dinitrotduene (71 ), 1.34; 1.3.5
and 1.2.6
Trinitrotoluene (82^
Isopentane Qess than —24^
• • •
T
• • •
(Bramley. 19x6.)
-13s
80.2
rKremaxm and Rodinis, 1906.)
-18.7
74. 2 »
u «
-17. s
86.8*
(1
- 7.3
94.5"^
(Kremann, X906.)
-13 ,
86.5"
t«
not determined
((Kiemann and Rodinis. X906.)
-17
89
(Kremann, 1904.)
-13-
80.8
(Kremaim. X906.)
- 8
96.4"
(Campetti and dd (jrosBO. X9Z3*)
> A second eutectic nlelts at 76* and contains 7 per cent (^H|NH|. a molecular compound of m. pt 93*
and containing 34 per cent C«H|NH| exists between these eutectics. The author also gives data for the
effect of nitrobenzene. 0 nitrophenol and of m xylene upon the lowering of the m. pt. of the above oom-
poond. * A break in the curve at 4X.5* and 39.3 per cent C^Ht!^ indicates that a molecular compound
exBts 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 5 trinitrobenzene (m. pt. 30*) exists over
the range pure aniline to the second eutectic which melts at xox** and contains 8.7 per cent C^HiN^.
* A second eutectic melts at o and contains 38.7 per cent CtHiNHa, the molecular compound between
these points mehs at 8.3* and contains 46.3 per cent (]«H|NHt. ■ A second eutectic melts at — 3x* and
contains 17 per cent C|H|NHb the molecular compound between these points melts at — X4.6* and con-
tains 49 per cent C^BcNHs. * The second eutectic melts at 6* and contains 33 per cent QHiNHf, the
molecular compound melts at X9.3* and contains 47.5 per cent CtHsNHt. ' There are two eutectics
between' which an equi-molecular combination exists. * There is a break in the curve at 36* and 43 x.
per cent C«B«NHf indicating the existence of a molenilar compound from the eutectic up to this point.
» There is a break in the curve at 43* and 39.8 per cent C^H«NHs indicating formation of a molecular
compound. >* There is a break in the curve at 74* and 33.9 per cent CJEUS^t indicating the existence of
a molecalar compound from the eutectic up to this point. ^ There is a break in the curve at 39* and
48.9 per cent C«H»NI^. ^ A second eutectic melts at 60* and contains 7 per cent C(H6NH|« the moleo-
ohr oompounds melts at 85* and ccwitains 30 per cent (VH«NH^
ANILINE 78
REaPROCAL SOLUBILITT OF AnILINB AND HSXANB.
(Keyes and Hildebrand, 19x7.)
t" cli Complete
Gms. Hez&ne per 100
V of Complete
Gms. Hezaoe per zoo
Misdbility.
Gms. Mizture.
MJadbUiV.
Gms. Miztuxe.
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
S1.4
21
53.9
731
S6
27.2
47.2
80.6
58.2
31
35-6
88.1
58.2
34.6
16. s
93-8
RsaPROCAL S(M.UBILITY OF AnILINB AND PhBNOL, DBTBRMINBD BT THB
Freezing-Point Method.
(SchreiiiemakerB, 1899.)
Mols. CHiNH, Mob. C«ILNH,
rofMeltiAg.
per zoo Mols. Solid Phase.
Mizture.
r> of Melting.
per zoo Mols.
Mizture.
Solid Phase.
- 6.1
100 CiHiNH,
30.4 m.
Pt
50
I.x
— 8.9
96
28.6
40
«
— ii.7Eutec.
92.3 C,H.NH,+x.i
22.3
30
M
" 6.5
90 i.x
14.8 Eutec.
21.2
z.z+C|H^H
+10.1
80
18.4
20
CiHdOH
22
70
31.4
10
M
28.5
60
37.3
4
U
I.I - C«H,NH,.CJiiOH.
Data for* the solubilitv of aniline in cyclohexane at pressures up to 300 at-
mospheres are given by Kohnstamm and Timmermans C1913).
ANILINE HTDBOCHLOBIDE C«H»NH,.Ha.
100 CC. H2O dissolve 17.8 gms. of the salt at 1 5°. (Niementowski and Rosskowski, 1897.)
100 gms. HsO dissolve 107. 1 gms. of the salt at 25°. (peddle and Turner, Z9Z3.)
100 gms. sat. solution in water contain 52.1 gms. C«HfNHi.HCl at 25**.
100 gms. sat. solution in aniline contain 8.89 gms. CeHtNHs.HCl at 25^
(Sidgwick, Pickford and Wilsden, Z9zz.)
Distribution of Aniline Hydrochloride between Water and Aniline at 25^
(Sidgwick, Pickford and Wilsden. z9zz.)
O.II
0.006
19.30 0.6 0.219 2.74 I 0.804 1.24
0.2
0.3
0.4
0.5
0.020
0.043
0.086'
0.146
10 0.7 0.327 2.14 I.I 1.005 I
6.98 0.8 0.471 1.70 1.2 1.228 0.98
4.65 0.9 0.631 1.43 1.3 1. 412 0.92
3 42
line layer
gms. salt
per 100 gms. aq. layer. C. — gms. salt per 100 gms. ani-
Nitr ANILINES
C.H4NHaN0,. 0, m, and p.
Solubility in Water.
— J. Chem. Soc. 53* 76S. '88; Vaubel — J. pr. Chem. [a] 5a, 73. '9S1 Abovv M^»
LOwenherz — 2. physik. Chem. a& 407, '98.)
f.
30
24.2
" Grams Nitraniline per Liter of Solution.
Ortho Nitraniline. Meta Nitraniline. Para Nitraniline.
I.I4-I.67 0.77-0.80
1.25 (25*^) 1.205
27 .1
... I •422 ...
100 CC. HsO dissolve 2.2 gms. P nitraniline at lOO^ (Jaeger and Kxegten, I9xa.)
79
NitrAHILniU
SOLUBIUTY OF OrTHO AND 07 MeTA NiTRANILINE IN HYDROCHLOSIC
Acid.
(LowmheR.)
Ortho Nitraniline at 35^.
G. Mds. per Liter. Grams per liter.
^ QUcNtf.. HCT
O-O
0.63
0.9s
1.26
0.0091
0.0143
0.0174
0.021);
CaUiNHs.
NQ,(o)
0.0 1.25
22.97 1.97
34.63 2.40
4';-94 a -97
(250) 0.0
(26.5®) 0.0125
(23-3*') o- 0247
Meta Nitraniline.
G. Mob, jper Liter. Grams pgr Liter.
HCl GiHsNH.. rfa CbUsNH^
CsHsNHs.
NOs(m)
0.0091
0.0183
0.0274
0.0
0.46
0.90
1.20
2.53
3-85
SoLUBniTT Data Determined bt the Freezing-Point Method Are Given
FOR the Following Mixtures.
0 Nitraniline + m Nitraniline
0
«
+ P
m
u
+ #
0
ii
+ 0 Nitracentanilide
P
«
+ p Nitrosoaniline
0
«
+ Benzene
M
«
+ "
P
41
+ "
0
it
+ Nitrobenzene
m
l<
+
P
fi
+
0
<l
+ Ethylenebromide
m
tt
+
P
U
+
Iff
tt
+ Iff Dinitrobenzene
Iff
<c
+ s Trinitrobenzene
P
<l
+ s
Iff
<4
+ Naphthalene
0
«
+ Phenol
m
14
+ "
(Kxcm«m, 19x0; Valeton, 19x0; HoQeman, JTi^Ttngt
and van der Unden, X9xx, Nicbds, X918.)
(Jaeger, 1906.)
(Jaeger and van Kiegten, 19x2.)
(Bofojawlensky, ^nnogxadoir and Bogalubow, 1906.)
«
«
M
M
M
«
M
«
M
M
U
M
«
M
M
M
M
M
M
M
M
(Crompton and Whitely, 1895.)
(Smith and Walts, 19x0; Sudboxoogh and Beaid, X9xa)
<i
II
i<
u
(Pushin and Grebensdukov, X913.)
(Kitmann and Rodinis, X906.)
II
M
II
P " +
s Tribromaniline + a Chlor, 4.6 Dibromaniline (Sudborough and T^khamalani, 1917.)
P Nitroethylaniline + p Nitro8oethylaniline (Jaeger and van Kiegten, xgxa.)
P " propylaniline + p Nitrosopropylaniline "
Nitrodiethylaniline + Nitroeodiethlyaniline aa««er. x9os, X907.)
Methylaniline + Benzylchloride (Wioc^ynski and Guye, x9xo.)
Dimethylaniline + Benzene (Schmidlin and Lang, x9xa.)
+ Tetramethyldiaminobenzophenone
+ Phenol
+ 0 Chlorophenol
Tetranitromethylaniline + a Trinitrotoluene
" -j- P Nitrotoluene
Nttnosodimethylaniline + fi Naphthylamine
+ Phenol
+ 0 Toluidine
+ /> "
+ Iff Xylidine
II
II
ti
tt
It
M
(Bnunley, 19x6; Kremann, 1906^
(Bramlcy, X9x6.)
(Giua, X9X5.)
II
(Kxuoann, 1904.)
NitrANnJNX
80
Solubility of Meta and of Para Nitraniline in Organic
Solvents at 20°.
(Canelly and Thonuan.)
Cms. per liter.
Sdvoit.
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Iso Butyl Alcohol
Iso Amyl Alcohol
Ethyl Ether
MeU.
II0.6
70
S6
26
78
5
5
4
I
9
Para.
95-9
S8-4
43S
19. 1
62.9
61.0
SoiTeot* •
Benzene
Toluene
Cumene
Chloroform
Carbon Tetra Chloride
Carbon Disulfide
Gns. |xr liter.
MeU.
Para.'
24. s
19
.8
17. 1
13
.1
" s
9
0
301
23
.1
2.1
I
■7
3-3
2
.6
ANILIME SULFATB CJItNHs.HtSOf,
100 cc. H«0 dissolve 6.6 gms. C«HfNHs.HiS04 at 15"*.
(Niementowski and Roedtofwaki, 1897.)
ANISIC ACID (^Methoxybenzoic Add) CHiO.CtHiCOOH.
1000 cc. sat. aqueous solution contain 0.2263 S™. acid at 25**.
(Paul. X894.)
Solubility op Anisic Acm in Several Alcohols.
(Timofeiew, 1894.)
In Methyl Alcohol. In Ethyl Alcohol.
Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sol. Solvent. Sat. Sol. Solvent.
o 51.1 104.5 4^-7 ^7-^
16. s 64.9 183.5 53-6 115. 5
r.
In Propyl Alcohol.
Gms. per 100 Gms.
Sat. Sol. Solvent^
35 53.8
43 7SS
Data for the distribution of anisic acid between water and olive oil at 25*
are given by Bo^seken and Waterman (191 1, 1912).
^ANISIDINE C6H4(OCH,).NHs.
Distribution between Benzene and Water at 25^
(Farmer and Warth, 1904.)
Gms. QH4<0CHa).NHa per loo cc
(}cH« Layer.
0.4356
0.6662
H«0 Layer.
0.0747
O.III2
0.9010 0.1472
AMISOLE C.Hg(X:H|.
Reciprocal Solubility of Anisole and Benzyl Chloride Determined
by^ the Freezing-point Method.
(Wroczynski and Guye, 1910.)
f ol
Melting.
-37-2
-40
-50
-60
Gms. CiILpCH« CqIjj
per xoo Gms. pu«!^
fof ^
Melting.
ICX) 04^X3,
— 72.8Eutec.
93-3
-60
75.3
-50
62.1
-41. 1
Solid
Phase.
Gms. CJIipCHi
per 100 Gms.
Mixture.
46 . 1 C»H|0CH,+(VH«(3^
28 C|H»CHta
13
o
M
^ NitrANISOLE C«H4N0s.0CH,.
Freezing-point Curves (Solubilities, see footnote, page i) Are Given for
THE Following Mixtures.
P Nitranisole + Mercuric Chloride (MascareUi, 1908, 1909; MascareUi and AscoU, 1907.)
-j- Urethan (Mascarelli, 1908, 1909; Pushin and Gxebeoachukov. Z913O
+ " + HgCli (Mascarelli, 1908, 1909.)
4- Diphenylamine (Pushin and Grebenschukov, 1913.)
Dinitranisole + Dinitrophenetol (Blanksma, z9X4-)
II
11
8l
ANTHRACENK
MMTBBACBXE C14H10
SCX^UBILITT OF
Anthracene in Several Solvents.
SolveDt.
f.
.ScnSl^lSJSt. Authority.
Etfiyl Alcohol (abs.)
16
0.076
(v. Becchi.)
« ti li
19. S
^.9
(de Brayn, xSga.)
tt it tc
25
0.328
(Hildebnuid, ElleCaon and Beebe, 19x7.)
it l€ (C
b. pt.
0.83
(v. Becriii.)
Methyl Alcohol (abs.)
195
1.8
(deBrusm x99a )
Benzene
25
.1.86
(Hildebrand, EUefson and Beebe. 19x7.)
Carbon Disulphide
25
2.58
M «• M
Carbon Tetrachloride
25
0.732
fi M M
Ether
25
1.42
M M M
Hexane
25
0.37
M M a
95% Formic Add
18.3
0.03
Toluene
16.5
0.92
(v. Beochi.)
(t
100
12.94
M
Trichlorethylene
15
1. 01
(Wester and BniinA, 1914.)
Solubility of Anthracene in Benzene and in Mixtures of Benzene
and Pentane and of Benzene and Heptane.
Ciyrer, x9xo, and private oommiinication. See Note, p. 447.)
In Benzene.
In Benzene + Pen-
tane at 15'
In Benzene + Heptane
at 14** and 70*.
Gns. CuHm
Gms.
O
10
40
SO
60
70
75
d. of Sat. SoL per 100
SotvciU.
0.605
0.975
1-43
2.03
2.78
3-75
514
7
8.35
in Sot
vent.
Gms. CuHio
per xoo Gms.
Solvent.
%CAin
Sol
vent.
Gms. QHm per 100 Gms.
~ Went ■
^\
atx4*. at7o^'
o 0.184 o 0.210 1.67
10 0.225 12.^ 0.284 2.10
20 0.279 25 0.372 2.64
30 0.357 37.5 0.474 3.23
40 0.447 50 0.592 3.87
50 0.549 62.5 0.718 4.59
60 0.600 75 0.850 5.37
70 0.780 87.5 0.976 6.15
80 0.915 100 1. 180 6.93
90 1.059
100 1.225
Results for the solubility in benzene, differing from the above in some cases by
15%, arc given by Findlay (1902).
Solubility op Anthracene in Alcoholic Picric Acid Solutions
AT 25^
(Behxend — Z. phyiik. Chem. Z5» x87* '94O
0.9008
0.8909
0.8812
0.8717
0.8627
0.8541
0.8460
0.8374
0.8347
Gnms pcf too Gfams
*Sdti
ution.
Kcric
Acid.
O
1. 017
2.071
2.673
3 233
Anthracme.
0.176
0190
0.206
0.215
0.228
SoHd
Grams per xoo Gms.
Solution.
3 .469 o . 236
Anthracene
u
it
tt
Anthracene and
Anthracene Picrate
Picric
Add.
3-999
S087
5-843
6.727
75"
Anthracene.
0.202
0.180
0.162
0151
0.149
7-452 o
Solid Phase.
Anthracene Picrate
it
it
tt
Anthracene Picrate
+ Picric Acid
Picric Acid
ANTHRACENE
82
Solubility in Liquid Sulfur Dioxidb or IHB Critical Region.
(Centneraiver and Tdetow, 1903.)
Weighed amounts of anthracene and liquid SOt were placed in glass tubes
which were sealed and rotated at a gradually increasing temperature, and the
point observed at which the solid disappeared.
r.
Gms CmHm per
100 Gms. SOb.
r.
100 Gms. SCV
r.
Gms. CmHio
xoo^.Gms. S
40.1
2. II
6s
4
98
9 36
45-8
2.48
78. a
S.66
99.1
995
47-9
2.6s
88
7.14
106.5
12.78
Freezing-point curves are given for mixtures of anthracene and each of the f<A*
lowing compounds: Diphenyl, diphenylamine, a and fi naphthylamines, a and fi
naphUiols, resordnol, p toluidine and triphenyl methane (Vignon, 1891)^ Naph-
th;uene (Vignon and Miolati, 1892); Phenanthene (Vignon, 1891, Garelii, 1894);
Picric acid (Kremann, 1905).
V.
30
Si-5
67.9
82.4
per
ANTHRAQUINONE (CJIOtCCO)..
Solubility in Liquid Sulfur Diozidb in thb Critical Rbgion.
(Centnenwer and Teletow, 1908.) (See Anthracene, above.)
Gms. CuHA pa *• Gms. Ci4H^
zoo Gms. SCV. * * 100 Gms. S
0.64 92.1 2.81
0.88 IOI.4 3.67
1.73 106.3 4.23
2.24 108.7 4*40
118. s
141. 6
160
179
183.7
G1118.C11HA1M
100 Gms. SOp.
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 p£Lrts at b. pt. (v. BeochL)
.100 gms. alcohol dissolve 0437 gm. anthraquinone at 25**.
(Hildebtand, EUeCBon and Beebe, 1917.)
Solubility of Anthraquinonb in Benzene and in Chloroform.
(!>!», xgio.)
In Benzene. In Chloroform.
^ A ^
«•.
Sp. Gr. Solution.
Gms. CuHAper
0
0.8900
O.IIO
30
0.8794
0.256
30
0.8692
0.350
40
0.8591
' 0.49s
so
0.8439
0.700
60
0.8389
0.974
70
0.8288
1. 355
80
0.8190
1.775
r.
Sp. Gr. Solution.
Gms. CmH«Pi per
xoo Gms. CHC1|.
0
1.5244
0.340
10
1.5046
0.457
20
1.4850
0.605
30
1.4656
0.780
40
1. 4461
0.994
50
I. 4261
1.256
55
I. 4164
1. 415
60
1.4070
1.577
Solubility jOF Anthraquinone in a Mdcturb of Chloroform and
HSXANB AT 12.6^ AND 49^.
(TVrer, 1910, also private crnnmuniration. See Note, p. 447.)
%CHCl|in
' Solvent.
O
10
20
30
so
Gms. Ci^A per 100 Gms.
solvent at:
12. 6*. 49-0.
0.006 0.056
0.016 0.074
0.024 0.096
0.034 0.124
0.068 0.212
%CHa|in
Solvent.
60
90
100
Gffls. C|JIA per xoo Gms.
Solvent at:
xa 6«.
O.IOI
0.148
0.222
0.334
0.482
490*.
0.292
0.417
0.608
0.852
1.209
83 anthbaquinomb
Solubility op Anthraquinonb in Ethbr.
(Smits— Z. Electiocfaem. 9$ 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 diown. The following figures were read from the curves, and
are therefore only approximately correct.
Gm9.CiA0!i
Cms. CuHM
. ^
GniB. CuHigOi
t*.
per xoog.
t».
per xoog.
Salnticn.
t*.
ner xoog.
Sohitkn.
130
3
241
30
260
80
ISO
4
245
40
270
90
170
45
247
SO
27s
100
19s
S-o
250
60
100 parts of toluene dissolve 0.19 part anthraquinone at 15° and 5.56 parts at
100* (v. Beochi).
100 gms. ether dissolve o 104 gm. anthraquinone at 25^.
(Hildebcand, EUefwn and Beet)e, 19x7.}
Data for the solubility of anthraquinone in mixtures of phenol and water
are given by Timmermanns (1907}.
Hydroxy ANTHBAQUIN0NE8 C«H« < (CO)t > CeH,OH.
1000 cc. H/y dissolve 0.0035 gm. a oxyanthraquinone at 25^ (Hfittig, Z9X4«)
1000 cc H^ dissolve o.ooi i gm. fi oxyanthraquinone at 2^^ "
1000 cc. H«0 dissolve 0.000012-0.000062 gm. 1.4 dioxyanthraquinone (« chin-
izarin) at 25^
1000 cc HiO dissolve 0.00158 gm. 1.6 dioxyanthraquinone ( » chrysazin) at 25^
(HQttig, 1914.)
ARTHRAFLAVINE (2.6 Dioxyanthraquinone) CuH«(CO)s(OH)s.
1000 cc H^ dissolve 0.0003 gm. anthraflavine at 25^. (HQttig, 19x4.)
AHTH&ABUFnVE (1.5 Dioxyanthraquinone) CuH8(C0)s(0H)s.
1000 cc H«0 dissolve 0.000285 gm. anthrarufine at 25^ (Hattig, 19x4.)
ANTIMONY Sb.
Fusion-point data for mixtures of antimony and iodine are given by Jaeger
and DcnmDosch (1912); for mixtures of antimony and sulphur by Jaeger and
Van Klooster (1912), and for mixtures of antimony, iodine and arsenic by
Querc^h (1912).
ANTnCOinr XriBBOMIDE SbBr,.
SoLUBiuTy IN Benzbnb Dbtbrhinbd bt " Synthetic Method.'*
(Menschutkin, 19x0.)
Gms. SbBri
Gim. SbBri
t". per 100 Gnu.
Solid Phase.
r.
per zoo Gms. Solid Phase.
Sat.SoL
SatSoL
5.6 m. pt. 0
CA
90
83 aSbBri.CA
4 . S EuteC 8 . 3 CA+aSbBr,.CA
92 . 5 m. pt.
90.2
IS ".5
aSbBra.r«Il«
91. S
92.8
35 23
w
90
93.8
SS 39
«
85 Eutec.
96.3 aSbBri.CA+SbBri
75 60.5
II
90
98 ShBra
85 74.3
m
94
100
ANTIMOinr TriBBOMIDE
84
Reciprocal Solubilities of Antimony Tribromidb and Various
Organic Compounds, Determined by the "Synthetic Method."
(Menschutkin, 1911.)
SbBri + Aoetk SbBri + Benzoic
Acid. Acid.
SbBr« + Benzoyl SbBri + Benzene
Chloride. Sulphonic Acid.
I Cms. SbBra
t*. per xoo Gm.
I Sat.SaL
52. S* o
SO 15.8
475 26.2
44 1 36.9
50 39.1
60 45-7
70 55.2
80 68.1
85 77.6
90 90.3
94 100
Molecular compounds are not formed in the above systems. The diagram in
each case consists of two arms meeting at the eutectic.
Cms. SbBri
Gms. SbBri
Gms. SbBra
r.
perzooGma.
r.
per 100 Gma.
t*. perxooGma.
Sat. Sol.
Sat.SoL
SaLSoL
16. s*
0
120*
0
— O.S* 0
IS
12.3
"5
30. z
- 3^ 195
xo
41. 8
no
36.8
- 6t 32
4t
58.3
105
SO
+10 41.3
30
64.3
100
61. s
20 47. 5
40
72. s
95
71
30 54
60
8Z.9
*5.
83.1
40 60.8
70
97.1
79 1
87.6
SO 67.8
80
93.4
85
92
60 74.9
90
97.8
90
96.4
80 89.4
94
100
94
100
94 100
SbBri + Acetophenone. SbBri + Amylbenzene. SbBri + Anisole.
CiHtCOCEta
4f
M
19. S* o
15 22.7
1. 5* 48.6
20 s6-8
30 63.3
37.5* 75
3it 83.2
40 84.6
60 88.4
(80 94.1
194 100
+I.X
Z.X
If
M
z.i+SbBrg
SbBrs
i<
M
If
If
Gms. SbBfi Solid
t*. per xoo Gms. i>i»-^
Sat. Sol. ^*"**-
—70 4-5 SbBr|.CeH*.C»Hu
-50 8.3
—30 16.6
— 25 21
^17 t 32. S "+SbBri
— 10 33. S SbBr,
o 35-6
20 41 . 6
40 51.3
60 6s
80 84
II
II
If
Gms. SbBri C/jwi-
*•• "^sit^sS""' p^
o CAOCH^
2.S "+I.I
II. 7 I.I
26.5
371
50.5
59
-34*
-35
— 20
o
10
20
25
M
«l
II
M
II
30.5* 77
30 1 77-9 "+SbBr|
40 80.6 SbBra
60 86.4
80 93.6
If
u
SbBri + Benzaldehyde. SbBri + Benzonitrile. SbBri + Benzophenone.
^' P^fJ^^S""- Phase.
-20
o
20
35
40
41.5
Sat. Sol.
38.4
455
54.3
64. z
70.3
77.3
1.1
II
fi
M
M
II
fl
11
37.8 1 84.4 z.i+SbBrg
55 88 SbBra
75 93.1
8s 96. z
90 98.3 **
94 100 • "
* m. pt.
f.
•13.2
-16
■18 1
o
30
30
38;
35 t
55
75
85
90
94
Gma. SbBrg Cfjtjfi
^sit^sS™- ^^^
♦ 0.0 CHaCN
19.2
If
28.7 "+1.1
43
59
67
.77.8
82. S i.i+SbBra
87. S SbBra
93.3
96.5
98.3
100
t Eutec.
I.X
II
II
If
If
II
Gms. SbBra c-i;<i
48 * O CaHaCO.CaHi
40 24
29 1 41-2 "+1.1
40 SO x*x
45 ^56.3
48.s*66.4
45 ' 76
40 80 i.i+SbBik
SO 82.6 SbBra
70 88.7 "
80 92.4 **
90 97.3 "
94 100 **
t tr.pt.
I.I » compound of equimolecular amounts of the two constituents in each case.
85
ANTIMONY TriBBOMIDE
^BCiF&ocAL. SoLUBiLjnBs OP Antimont Tribromidb and Various Organic
Compounds, Dbtbrmined by thb "Synthetic Method."
(Menachutkin, 1910.)
SbBrj
le-
SbBr, -f
SbBr, +
SbBr, +
Brombenzeiie.
Chlorb^zene.
lodobenzene.
Fluorbenzene.
{
ctins. SbBra
Gms. SbBrg
Gms. SbBra
Gms. SbBr,
IT. per 100 Gms.
r.
per 100 Gms.
t*. per 100 Gma.
t*. per 100 Gma.
Sat.SoL
SaLSoL
Sat.SoL
Sat.SaL
-31 •
0
-45.2*
0
-28.6* 0
-39.2* 0
-32^
S-7
-47 1
S-2
-30.3 7.0
-32? 14.3
-39. st 1.3
-25 1
95
-40
6.8
-25 4.3
-15
IS
-30
9.6
— 20 21.6
-15 6.7
- S
20.8
— 20
Z2.6
— 10 27.5
+ S 12.6
+ S
26.8
—10
16
. 0 33.4
25 21.8
IS
33
0
20
+10 39.3
45 35-3
25
39-6
20
30
20 45 . 2
SS 4SS
45
S4-6
40
45-4
40 57-6
6s 60.8
6S
71.9
60
65.8
60 71. I
75 81.8
8S
90.7
80
86.3
80 86.3
85 93S
94
xoo
94
100
94 100
94 xoo
SbBr,+
SbBr, +
SbBr, +
SbBr, +
p Dibrombenzene.
p Dichlorbenzene.
Nitrobenzene.
tn Dinitrobenzene.
Gms. SbBra
Gms. SbBri
Gms. SbBra
Gma. SbBra
r.
per zoo Gms.
f.
per 100 Gms.
t*. per zoo Gms.
t*. per 100 Gma.
Sftt.SdL
SatSoL
Sat. Sol.
Sat. Sol.
88*
0
S4S*
0
6* 0
90* 0
8S
10
Si-S^
14
Z 22
80 29. z
80
25.2
48.st
26. s
- 4 37.4
70 SO
7S
39-2
S5
35 9
- 9 48.4
60 63
70
52
60
431
-i4St 553
SO 70.8
6st
62.2
6S
SO. 7
- s 58.3
. 47. st 72
70
68.7
70
S8.8
+ S 61. s
SO 73-4
7S
753
7S
67.2
25 68.6
60 78.2
80
81.8
80
75-8
45 76.6
70 84
8S
88.3
8S
84. S
65 85.3
80 90.4
90
94.3
90
93.4
85 94.7
90 96.8
94
100
94
100
94 zoo
94 zoo
Molecular compounds are not formed in the above systems. The diagram
in each case consists of two arms meeting at the eutectic.
SbBr,
+ Ethylbenzene.
SbBr,
+ Propylb
enzene.
SbBr, + p Cymene.
r.
JS^Jf^ Solid
f.
Gma. SbBra
per xoo Gma.
Sat. Sol.
Solid
Phase.
Gma. SbBra
t*. per xoo Gma.
Sat. Sol.
Solid
Phase.
-93*
0
C|Ht.CiHa
-80
1-3
X.I
-7S* 0
-93.2'
\ 0.4
"+Z.X
-60
3-7
ti
-77 1 2
-70
z
Z.Z
-40
9.4
II
—50 6.Z
1.1
-SO
2.2
t«
—20
22.5
M
—30 12.3
w
-30
4.8
cr
— 10
38.4
M
— zo 27
a
— 10
Z2
n
- st
49 x.z+SbBra
0 42.3
M
+10
29.2
M
+10
S3. 3
SbBr,
+st S^S
x.z+SbBi|
20
46.3
II
20
S7.I
M
20 56
SbBfk
29t
69.7
i.z+SbBr,
40
66.2
U
40 64. z
M
50
78.2
SbBra
60
77.2
M
60 75
a
70
87.3
«
80
89.8
a
80 88.5
■
90
97.7
II
94
zoo
M
94 zoo
«
m. pt.
t Eutec.
t tr.pt
I.I » compound of equimolecular amounts of the two constituents in each case*
ANTIMONY TriBBOMIDE
86
Reciprocal Solubelities op Antimont Tribromidb and Various Organic
Compounds, Deterionbd by the "Synthetic Method."
(Menacbutkin, 191 x.)
SbBfi + Cyclohexane. SbBri + Pseudo Cymene. SbBrt + Mesityleoe.
Gms. SbBra CqIm
t". per 100 Gnu. pi,.^
Sat. Sd. *^°*"-
6.4* o CiHb
6t 0.3 C|Ha+SbBr,
20 1.4 SbBrg
40 3-7
60 7.1
80 12.5
liquid layers formed
92.5 17.4 97.6
no 25.8 96.5
130 36 -4 95
150 47.8 92.7
170 62.3 86.3
175 1 74.0
i<
If
u
Gms. SbBra c^ka
V. per 100 Gms. ,5?"°
-57.2* o CaHi(CH,)i,a,4
-58. 8t 9.7 " +"
— 50 II i.x
—30 16.2
— 10 31
o 47.6
7 5 63.5 x.z+a.i
15 67.4 a.i
25 73
338 791 a.x+SbBr,
50 82.8 SbBr,
70 88.4
90 97.4
Gms. SbBri
t*. per zoo Gms.
Sat. Sol.
Solid
Phase.
M
M
If
ff
ff
-54.4* O CA(CH|)sX.3.5
— 5S.2t 2.1 " +IX
—30 3.6 x.x
— 10 9
+10 25.4
20 35-5
29; 46.5 i.x+a.x
40 54-2 a.x
50 61.7
60 70.2
69.5*85.8
69 1 87.7 a.x+SbBrs
80 92 . 7 SbBtg
tf
ff
ft
tf
ft
it
SbBfi + Diphenylmethane. SbBfi + Naphthalene. SbBfi +a Nitronaphthalene.
Gms. SbBri
V. perxooGms.
Sat. SoL
SoUd
Phase.
26*
22. 5t
40
50
60
70
80
90*
82 t
90
94
o
12.8
22.8
295
37.5
47.8
60.2
81. 1
89.6
92.2
96.2
100
CH,(CA)t
"+a.x
a.x
a.r+SbBri
SbBra
ti
Gms. SbBrg CnH/i
f. per 100 Gms. ^^
Sat. Sol. '^*«»»-
79.4 *
75
70
65
57
60
66*
65 t
75
85
90
Gms. SbBr* c^uj
r. per 100 Gms. ^^^
Sat. Sol. ^^^^'
0
CuHg
57*
0.0
«C,.H,NOi
237
(f
50
23.2
(f
37.4
(f
40
42.6
ft
48.6
ft
33-5t
50. 5
"+1.1
61.2
" +a.x
37.5
62.6
x.it
68
a.x
38.2 •
67.6
If
81.3
if
38 t
68
x.x+SbBrg
84.9
ft
50
73.4
SbBrg
86.7
a.z+SbBra
70
83.8
ft
90.1
SbBri
90
96.4
M
94.9
u
97.7
ft
SbBri + Diphenyl.
Gms. SbBrg
t*.' per 100 Gms.
Sat. SoL
f70.5*
60
47 t
55 ^
60.5*
70
80
90
94
o
35
54
57
68
82
86
91
97
xoo
7
3
4
5
7
5
5
3
Solid
Phase.
CgHgCgHg
ff
If
If
+a.x
a.x
If
SbBr,
ff
If
tf
SbBri -h Phenol,
f ^r"?l;«^r^ SoUd
41 • o
35 22.5
30 40
28.5 t 44.6
40 53
50 62.5
60 75.8
65 84.7
66.5* 88.5
75 91-7
^85 95.8
90 98.1
CgHgOH
If
If
"+a.i
a.x
fi
ft
ft
SbBr,
ft
ft
SbBri + Phenetol.
Gms. SbBrg ^tAid
t*. per 100 Gms. pj^
Sat. Sol. ^°*"-
-28.6* o CgHiOCiH.
-29 1 1.6 " +I.X
— 10 4.8 x.x
+10 12.9 "
20 19 . 2 **
30 29.7 **
40 46.2 "
48.8* 74.7
47 1 77.8 z.x+SbBx|
60 83 SbBrg
70 87.3
90 97.4
ft
* m. pt. t Eutec t crit. t. ( tr. pL
t Not obtaixied regularly, in such cases, single eutectic at aj* and 6x.s per cent SbBrg.
I.I =3 compound of equimolecular amounts of the two constituents in each case.
2.1 =» compound of 2 molecules of SbBri with one molecule of the other ooQ-
stituent.
87
ANTIMONY TriBBOMIDE
Recifsocal SoLUBiLmEs OF Antimont Tribromidb in Various Organic
Compounds, Determined by the "Synthetic Method.*'
' (Menscfatttkin, 19x0-12.)
SbBrj -{- ct Brom-
jsapfatlialene.
Gnus. SbBrs
t*. per zoo
Sftt. SoL
3"
o
— 3 si
35
45
S5
65
75
&>
85
90
o
3^ 7
49.9
56.9
64.7
8x.8
86.3
90.8
95-4
SbBr, + a Chlor-
naphthalene.
Gms. SbBra
t*. per xoo Gma.
Sat. SoL
-17*
— 21
— 24.St
— 10
+10
30
SO
60
70
80
90
94
o
13.8
32.6
27.3
35. S
46.7
61.6
69.9
78.6
87. S
96.6
100
SbBr, + /? Chlor-
naphthalene.
Cms. SbBra
V. per 100 Gms.
Sat. Sol.
S6*
SO
45
40
37. st
45
55
65
75
80
85
90
o
26.1
38.S
49
53-6
58.8
66.8
75.2
83.8
88.1
92.4
96.7
SbBr, -f Tetra-
hydrobenzene.
Gms. SbBra
t*. per zoo Gms.
Sat. SoL
-5
15
35
55
65
70
75
80
85
90
94
II. 7
15.1
24.1
41
55-1
64.5
76.2
84.4
90.7
95.8
100
SbBr, -h
0 Chlortoluene.
-38.st
—20
o
+20
30
40
SO
60
70
80
90
SbBr, +
m Chlortoluene.
10 -7
iS-4
32 -5
32.5
38-»
4.6. 8
66.5
77-8
88.3
97
r.
-47.8 ♦
— sot
—30
— 10
+10
30
40
50
60
70
80
90
Gms. SbBra
per xoo Gms.
dac doi.
o
8.1
II. 7
17.5
25.8
37.5
45- 1
54.4
65
77
88.2
97
SbBr, +
p Chlortoluene.
Gms. SbBr,
t*. per xoo Gms.
Sat. SoL
6.2*
2. St
20
30
40
50
60
70
80
90
94
o
23-3
33
39-3
47.2
56.3
66.7
77.8
88.2
97
100
SbBr, 4-
m Nitroluene.
Gms. SbBra
t*. per 100 Gms.
I Sat. SoL
16 ♦ o
10
5
o
- 9t
+10
30
50
60
70
80
90
24.2
39
46.6
56.8
62.7
69.7
77.5
81. 5
86.3
91.4
97.2
Moleculair compounds are not formed in the above systems,
each case con^sts of two arms meeting at the eutectic.
The diagram in
SbBrs + Toluene.
S555? Solid
Phase.
SbBr, -h 0 Nitrotoluene.
f.
-93' _
-93-5t
-80
—60
—40
— 20
- it
+20
30 t
40
60
94
I.I
2.1
Gms. SbBra
t^. per xoo Gms.
Sat. SoL
Solid
Phase.^
o
T .0
2.4
6.2
X2.4
25-7
53-1
69.4
80.6
86.6
93.8
PftH6.CHa
I.I
<f
M
M
X.I +2.1
2.1
2.1+SbBra
SbBra
.«
(I
- 8.5*
-13-5
o
10
20
25
31 1
40
50
60
80
90
* m. pt.
o
19. 5
27.6
35.6
47.5
55. 7
70
73.5
77.5
81.7
91.4
97.2
o N0|.C|H».CH,
" +1.1
x.i
(f
u
tt
" +SbBra
SbBra
u
u
M
CI
SbBr, -f p Nitrotoluene.
Gms. SbBri
V, per 100 Gms.
Sat. Sol.
SoUd
Phase.
t Eutec
52.5
45
40
35
16 1
30
50
60
70
80
90
X tr. pt.
O
29.8
42.2
50
61
67
71.6
78.9
82.9
87.2
92
97. s
p N0a.CaH(.CHa
+SbBr,
SbBr,
M
compound of equimolecular amounts of the two constituents in each case,
compound of 2 molecules of SbBr, with i molecule of the other con-
iirriMONY TriBBOMIDE
88
Reciprocal Solubilitibs op Antimony Tribromidb and Various Organic
Compounds, Determined by the "Synthetic Method."
(MeoBchtttkiii. 19x0-11.)
SbBr, + Tri-
phenylmethane.
SbBrt + 0 Xylene.
SbBri + m Xylene.
SbBr, + p Xylene.
r ^
Gms. SbBri
Gms. SbBri
Gnu. SbBri
Gnu. SbBra
r.
per 100 Gnu.
t*. per xoo Gnu.
f.
per zoo Gnu.
f.
per 100 Gnu.
Sat. Sol.
Sat.SoL
Sat. SoL
Sat. SoL
92*
0
— 29* 0
-57*
0
14*
0
8s
18
-33 t 10. S
-59. 2 t
55
12
16.6
80
30.1
— 20 17
-45
10
lot
28
70
47
— 10 24.6
-35
14.2
20
36
60
58.2
0 34. S
-25
20
30
44-6
48t
67.1
20 65.8
- S
38.8
40
53.8
60
73-3
24* 77.2
+ 5 ♦
56.6
50
63.S
70
79. S
22.5 t 78.6
12. St
75.4
60
74
80
86.4
30 80
25
77.6
67.5*
87.3
90
95-2
so 84.7
45
82.3
66.5 t
88.3
94
100
70 90.1
65
87.9
75
91.4
90 97.7
87 .
95.3
85
95-7
* m. pt.
t Eutec.
X tr.pt.
In the case of each of the above scylenes the compound existing between the
first and second eutectic consists of equimolecular amounts of SbBri 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. (Kuzakov, Krotkov and Okaman, 19x5.)
iirriMONT TriCHLORIDE SbCh.
Solubility in Water. Solid Phase SbCIa>
(Meerburg — Z. aaorg. Cbem. 53* 99Q> 1903.)
♦•.
Mols. Sbda
per 100
&iols.HsO.
Gnu. Sbda
per 100
g.HsO.
0
IS
47-9
64.9
601.6
815.8
30
25
30
572.4
(74.1
78.6
84.9
910. 1
931 s
988.1
1068.0
♦•.
Mok.Sbat
per 100
Mols.H|0.
Gnu. SbOa
per 100
g.HsO.
35
40
91.6
108.8
II52.O
1368.0
SO
60
3^-4
I917.O
4531 0
72
00
00
Solubility op Antimony Trichloride in Aqueous Hydrochloric
Acid. Solid Phase SbCl,. Temp. 20^
(liieerbais.)
Mols. per
100 Mob. HsO.
HQ.
O
2.4
6.1
8.3
SbCli.
72.4
71.2
69.9
68.2
Gnu. per
100 g. HjO.
BQ.
Mols. per
xoo Mob. HiO.
Gnu.
100
tu. per
g.HsO.
0.0
4.86
"34
16.80
SbOs.
910. 1
^95 -4
879.0
857.6
9.1
II. 7
28.7
SbOa.
68.9
68.1
62.8
fiS"
18.41
23.68
58.08
SbCla.
866.4
856.3
789.8
100 gms. absolute acetone dissolve 537.6 gms. Sbd at I8^ <2y sat. sol. = 2.2 16.
(Naumann, 1904.)
100 gms. ethyl acetate dissolve 5.9 gms. SbCh at 18"* d sat. sol. » 1.7968.
(Naumann, X910.)
89
iirriMONY TriCHLORIDB
Reciprcx:al Solubilities of Antimony Trichloridb and Various Organic
Compounds, Dbtermined by the ''Synthetic Method."
(Menschutkio, 1911.)
SbCU + Acetic Acid. SbCU + Acetophenone.
SbCh + Anisol.
Gma. SbQs Cnlvl
r. pcriooGms. ^£^
Sat-SoL
16.5* O
ZO
O
:|t
o
ID
25
45
65
73
22.7
42.5
48.S
52.7
59
67.3
•79.1
81.5
87.4
95.3
xoo
CHtCOOH
• tt
u
fi
" +I.X
X.X
u
it
SbCli
f(
u
If
r.
19s*
IS
ft
IS
35
55 ^
60.5*
32 t
SO
70
Gini.SbC]|
perxooGms.
SatSoL
Solid
Phue.
f.
Gms. SbOi Solid
per 100 Cms. p^^
O
14.3
28.5
31.8
35. 4
41.6
55-2
65.4
79-3
84
893
98.2
CACOCH.
II
M
+I.X
X.X
•I
II
M
x.x+SbCU
SbO.
-34*
-36.5 t
-30
— ID
+ 10
20
25 t
35 ^
41.5*
4ot
60
70
SatSd.
o
IZ.8
x6
28.3
43
52.8
63.6
70
80.9
845
92
98
CiHtOCH^
+X.I
II
X.X
M
a.x
w
+a.x
"+Sba,
SbOi
M
SbCla + Aniline.
Gms. SbOt
t". per 100 Gno.
Sat.SoL
- 7.2t
+20
60
77 t
88*
87 t
94. 5*
89-5t
too. 5*
70
31 1
60
X
7 -
18.7
29.6
44.8
46.3
54.9
61.7
71
82.2
88
94.9
SoUd
Phase.
CiH4NH,+x4
II
1-3
X^+X.3
X.3
x.a+x.x
X.X
II
x.i+SbCli
SbCU
SbCU + Benzaldehyde. SbCU + Benzophenone.
f.
xo
20
30
40
43. 5
40
25 1
35
45
65
73
Gms. SbCli CrtiM
perxooGms. w?^
"sat SoL ^*««-
43-5
47. 5
52.4
60.2
68.1
74.2
80.6
83
85
87.5
95-2
100
II
II
M
II
II
II
x.x+SbCl|
SbCU
II
II
Gms. SbCU
per 100 Gms.
SatSoL
SoUd
Phase.
48*
40
35 t
45
55
76*
65
391
50
70
o
16.3
21.6
26.2
314
37.5
55.4
71.6
80.6
82.7
87
97.7
CACOCA
11
+X.X
X.X
M
M
"+SbCU
SbOt
II
compound of equimolecular amounts of the two constituents in each case,
compound of 2 molecules of SbCU with i molecule of the other constit-
i.l
2.1
uent.
.1.2, 1.3 and 14 » compounds of i molecule of SbCU with 2, 3 and 4 molecules
of aniline.
Sbat + Benzoic
SbCU + Benzoyl
SbCU + Benzene
SbCU + Tetra-
Acid.
Chloride.
Sulphonic Acid.
hydrobenzene.
Gms. SbCU
'Gms. SbCU
Gms. SbCU
Gms. SbCU
t*. per 100 Gms.
t* per xoo Gms.
t*. per 100 Gms.
f.
perxooGms.
Sat.SoL
Sat.SoL
Sat.SoL
Sat. Sol
120 0
- 5 17.8
52.5* 0
-25
19. X
no 23
-15^ 36.8
45 18
-15
24
100 38.8
-23 1 45
25 43.7
- 5
30
90 so
- 5 50.7
5^ 56.1
+ 5
37.1
80 59
+15 58.2
-St 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
46t 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
73 100
65
92.8
Molecular compounds are not formed in the above systems. The diagram in
each case consbts of two arms meeting at the eutectic.
m. pt.
t Eutec
ttr.pt
iirriMONT TriCHLORIDE
90
SbCh + Brombenzene. SbCh + Chlorbenzene.
Gnu. SbCIt jn^;^
per 100 Gms. nu.-^
r.
RsaFROCAL SOLUBILITIBS OP AnTDIONY TrICHLOUDB AND VARIOUS ORGANIC
Compounds, DsTBRiaNED by thb "Synthbtic Mbtbod."
(MenschtttUn, igio-'ii.)
SbCh + Benzene.
Gms. SbOt s^y
I
10
20
40
60
79 1
70
62*
67. S
7.3 CA
19.4 " +«•«
24.6 9.Z
30- 5
44.1
60.6
76.8
85.3
93. 5
96 a.i+SbOi
97.9 SbO,
If
M
M
II
M
Gms* SbCU Sfllid
r. p^xoo (g^ p^.
-31 1 o CiHiBr
-32. 5* 4.8 "+I-I
—30 6.8 1.1
-20 14.8
—10 23.9 *•
o 34-3 "
+ 3 1 40.3 i.x+SbOi
20 52 SbCa«
40 68
60 85.8
73 100
-45. 2 t
-47*
-40
-30
-IS
-it
20
40
60
73
o
4.3
7
XZ.I
20.5
32. S
44.2
S6
72.1
88.2
TOO
CAa
z.z
M
M
II
II
SbCk + Fluorbenzene. SbCU + lodobenzene. SbCU + Nitrobenzene.
Giiis.^ai g^jj
Gms. SbCIa CqIm
Sat. SoL ^»««-
— 39.2t o CtHtf"
—40.5* 2.4 "+ 1.1
— 25 II
-IS 173
— 10 21.4
— S 26.4
o ^ 341
+ SSt 45-8 i.x+SbO,
IS S3-6 SbCU
25 61.6
45 77.7
;6s 93.8
z.z
M
II
H
II
II
II
Gms. SbCli g^uj
f*. per zoo Gma. m!^
-28.6 1 O CAI
-3S 12.8 "
-45* 29.8 "+Z.Z
—34.5 II. 7 z.z, unsUUe
— IS 26.4
— 3 .49.1
— 3S 32. S z-z+Sbd,
— IS 38.9 SbCI,
+ 5 46.4
25 56
45 69.6
65 88.8
II
i<
i<
II
II
r.
6t o CANOb
— 2 20.4 «
— 10 32 •*
-16.5* 38 "+Z.1
— lo.s 44 z.t
— 75 50
— 6t 64.8
— 6.5* 67.5 z-z+SbOi
+ 5 69.6 SbCU
35 78.7
55 87.4
70 96.6 •*
SbCh + Ethylbenzene. SbCU + Benzonitrile« SbCh + laoamylbenzene.
-93
-93
-70
-50
-30
—10
+10
30
39
35
37
36
50
70
33
Gms. SbOi Solid
, per 100 Gms. pKS
^st. SoL ^'*^-
"^ o C|H*.CA
.5* 0.3 "+"
0.6 IX
I.I
2.5
7
18.8
44.4
t 68.1
77.4 i.z+a.z
t 81. 1 az
.8* 81.8 a.z+Sba,
87.2 SbO,
98
M
II
II
II
II
li
f.
,Sr°Sl?rSj. Solid
per 100 ums. pu.-^
Sat Sol. ^'**-
13.2 t
16
19*
10
o
10
IS
20
o
10.2
17.2
21.9
28.5
38.7
47.4
62.6
80.4 z.z+SbCl|
^ (unstable)
* Eutec.
21. 5t 68.7
20 72.4
15* 78.9
25 81.6
45 87.6
65 95.6
73 100
tm.pt.
CACN
II
+Z.Z
z.z
II
M
II
II
•I
M
II
Gms. SbCU c^KJ
-80 4
—60 II. 7
-40 25.4
—33+ 32.7 z.z+aj
-25 38.7 a.z
-IS 47.2
— St 56.8 s.z+SbOs
o 57.4 SbOi
20 63.3
40 -72.6
60 .87.1 "
70 97.3
— 25 44.4 unstable Z.Z
— 21 t 54.9 "z.z+SbCU
— 10 56 "SbCU
ttr.pt.
Z.Z
II
II
14
M
I.I « compound of equimolecular amounts of the two constituents in each case.
2.1 s compound of 2 molecules of SbCh with i molecule of the other con-
stituent.
91
ANTIMONY TriCHLORZDE
Rbofrocal Solubilities of Antimony Trichloride and Various Organic
Compounds, Determined by the "Synthetic Method."
(Menschutkin, zqio-xi.)
SbCU + tn Dinitrobenzene.
r.
90*
80
70
60
SO
40
30
20
10
It
—II
+27. 5
28.5
27. 5
25
Gms. SbCli
per xooGms.
SatSoL
Soiid
Phaae.
O
18.6
40.7
48
S3. 6
S8
61 . 6 unstable
64. S
66.8
68.8
52.5
58.2
63
67. S
tt
M
tt
U
U
r. Peyoo a-., n^
72 . 8 unstable
76.2
M
U
C«H«(NQ|), 20
IS
10 78.6
S 80.8
o 82.7
— 10 64.9
+10 69
20 71.6
30 74.8
"+SbCl,40 78.7
SO 83. s
x.z 60 89
" 70 96.4
** 73 100
ti
x.z
«l
M
M
M
H
U
SbCli
It
CI
<l
M
CI
u
IC
SbCU + Propylbenzene.
Gnu. SbCIa
t*. per 100 Gms.
SatJ Sol.
Solid
Phase.
-70
-30
— 10
o
8.st
20
40
6S
• ■ •
-70
-30
- S ^
+ i.S*
it
10
0.6
10. 1
26.6
40.4
575
68.2
71.4
78. S
92. S
• • •
1. 5 »•«
16 "
48.2
65.3
66.3
68.6
9.x
M
M
••+sba,
SbOt
^iimtwMft
CC
c<
CI
M
fC
" +sbca, "
SbO. "
SbCU + p Dibrom-
benzene.
Gms.SbCli
per 100 Gms.
SatSoL
f.
88*
8S
80
70
60
ss
49St
6S
60
70
o
S.7
154
35
52.8
59
64
71.8
79-3
95
SbCU + p Dichlor-
benzene.
Gms.SbC]«
per zoo Gms.
Sat. SoL
f.
545*.
50
45
39St
45
SO .
55
60
70
14
30
48
50.S
59. S
67.8
75.7
83
96.2
SbCh + Cydohexane.
f.
Gms. SbCl« per xoo Gmt.
Sat. Sol
6.4* 0.0
6t o.a
20 1.2
40 4.2
60 9.7
Two liquid layers formed
70
80
100
120
124
125.58
13-7
19.5
32.3
57.1
58.9
68
97
96.1
92.7
83.2
76.7
SbCU + p Cyraene,
r.
Gnis.SbClt
per xoo Gms.
Sat. SoL
SoUd
Phase.
-75*
-76.st
-SO
-30
—10
- 3-5t
ID
30
4ot
SO
60
70
o
2
7
IS
30
41
46.1
60
76.4
81.2
87
95.6
P CACHiCH,
+X.X
<l
x.x
II
II
x.x+a.x
a.x
II
2.x+SbCU
11
If
•c
* nLpt
SbCh + Pseudocymene. SbCU + Diphenyl.
Gms. SdCI| GniSyi
P**«J~cS«*- Phase,
r.
Gms. SbCU
per TOO Gms.
Sat. Sol.
Solid
Phase.
-57. 4*
-60 1
-45
-25
— 10
- St
+15
35
50
56*
Sit
65
f Eutec
o
18.6
23.6
33.3
45
50.7
55.8
62.2
69.7
79.2
87.5
93.9
QHt(CH|),x,s,4
" +I.X
i.x
cc
H
"+a.x
+a.i
S.X
•I
S.X
il
II
11
s.x+SbOi
SbOi
t tr. pt
f.
Sat Sol
70.5* O CA.CA
65 14
55 33.4
40
45.2
SI.4
70.7 •*
74.6
85. 5
88.9 a.x+SbCli
93.1 SbCU
97
S exit. t.
sot
55
60
70
71*
57 t
65
70
II
I.I
3.1
compound of equimolecular amounts of the two constituents in each case,
compound of 2 molecules of SbCh with i molecule of the other constituent.
ANTIMONT TriCHLORIDE
92
Rbcip&ocal S(x.ubilities of Anthiony Trichloridb and Various Organic
Compounds, Determined bt the "Synthetic Method."
(Menachutkin, 19x0-1 z.)
SbCb + Mesitylene.
) Gms. SbCIa
per zoo Gms.
Sat. Sol.
Solid
Phase.
SbCU + Diphenyl
Methane.
Gms. SbCli
t*. per zoo Gms.
Sat. Sol.
SoUd
Phase.
-S4.4*
-55-6
-40
— 20
o
10
38 1
755*
70
58.5
63
70
o
IS
3
7
14.2
20.3
39-3
514
65.4
79.2
87
92.4
94
98
C|H|(CH.),z,3.5
+1.1
f<
X.I
(i
26*
22. St
40
60
70
80
90
+a.x 95
100*
95
90
+Sbai 80
SbOi 67 t
70
II
11
ft
tf
a.i
<i
If
«t
ft
o
7.9
15.1
26
33
41.6
52.7
59.8
72.9
8a. 2
86.7
91.5
95.7
97
CHe(CiHi)t
" +a.x
s.x
41
M
M
(I
U
11
11
M
<l
a.x+SbOt
SbOf
SbClj + Triphenyl
Methane.
Gms. SbClt
t*. per 100 Gms.
Sat. SoL
Solid
Phase.
92*
85
80
70
60
49T
45
40
35 t
45
55
65
70
o
II. 8
193
32
42.4
49.6
50
62.8
68.3
72
76.6
82.4
90.6
96.1
CH(CiH^i
ii
M
M
II
•I
" +I.I
x.z
x.x+SbCli
SbCl.
<i
ft
SbCk + Naphthalene.
Gms. SbCU
per zoo Gms.
siata 901.
SoUd
Phase.
;79.4*
75 .
59 t
65
75
80
86*
80
70
65 t
70
o
15. a
35
42.8
48.4
58.8
65
78
88.7
93
94
97.2
*<
(I
" +a.i
fi.X
If
If
fi
If
3.i+sba»
SbCIi
SbCU + a Chlor-
naphthalene.
Gms.SbCli
t°. per 100 Gms.
Sat. Sol.
QoHs —
SoUd
Phase.
21 t
O
10
20
30
40
46*
45-5 t
55
70
o
8.1
14.4
18.7
24.6
33-5
47.7
61. s
73-6
75
82.2
96.S
aCioHTQ
" +a.i
3.x
ft
fi
II
a.z+SbCli
Sbdi
fi
r.
56
50
45
40
30
25 1
29-5
28 1
35
45
60
73
SbCU + /8 Chlor-
naphthalene.
Gms. SbCU
per zoo Gms.
Sat.S<d.
Solid
Phase.
O
16.6
27.2.
35-4
47-3
52.3
58.2
64
68.3
75-3
87.5
100
^CiAQ
• +I.X
I.Z
x.z+SbCli
SbOa
•I
ft
ft
SbCh + a Bromnaphthalene.
f.
SbCh + a Nitronaphthalene.
10
25
33 ^
34.5*
33
31st
40
50
60
70
Gms. SbCIa per zoo
Gms. Sat. Sol.
O
8.3
12. 8
24
38.5
52.4
62.1
64.7
69.7
76.2
84.5
94.8
* m pt.
SoUd
Phase.
aCioHfBr
" +1.1
X.X
M
tl
x.x+SbCU
SbClt
I*
ft
t tr.pt.
Gms. SbCls per zoo SoUd
Gms. Sat. Sol. Phase.
57*
SO
^t
30 +
35
37.5
39*
37. 5^
34-5 t
45
60
70
o
136.
27.3'
35.8
43.2
49.3
56.7
64.9
72.8
78
87.4
96.6
X Entec.
a CjoHrNOk
«i
It
" +I.X
x.z
tl
u
s.x+SbCU
SbO.
I.I » compound of equimolecular amounts of the two constituents in each
case.
2.1 « compound of 2 molecules of SbCh with i molecule of the other con*
stituent*
93r
ANTDSONY TriCHLORIDB
Rbofrocal Solubilitibs op Antimony Trichloride and Various Organic
Compounds, Determined by the "Synthetic Method."
(Menachtttkiii, 19x0-13.)
SbCb + Phenol.
,£°^^r^ Solid
Sat.SoL
41'
35
30
20
xo
St
IS
30
37*
36.St
55
70
CAOH
M
U
M
" +a.i
o
16.2
25.6
38- 7
48
S2
58.6
70.6
83
83.7 a.i+SbCU
90.6 SbO.
98.2
M
M
SbCh + Phenetol.
f . per 100 Gms. ^J*2
-28.6*
-29 t
— 20
— 10
+10
20
30
40
42.2*
3St
SO
70
Sat. SoL
o QH^OCiHs
1-4
45
8.1
18.2
27.4
39-4
S8
65
77.8
86.8
97.1
•+I.X -
i.x
M
SbCh + Toluene,
f BS-"^^rSl Solid
93 • o CA.CH,
94 t I.I "+«•«
70 3.1 I.I
30 15.8
o 41. S
"t 57.8 "+a.i
20 62.8 S.Z
40 78
42. S* 83.1
40 1 8s. 8 a.i+SbOi
50 89 SbCU
70 97.8
f(
fi
M
U
«f
U
M
M
M
IC
«l
SbCli + 0 Chlortoluene. SbCU +|m Chlortoluene. SbCli + p Chlortoluene.
Gms. SbCif StJid
**• ""sTsS."- "—•
— 36.2* o oaC.H«CHi
-375 1 6.9 "+1.1
—20 18.3 I.I
— 10 29 . 2
- 5 ^ 37.1
- 0.5 1 47.9 i.i+SbCU
+10 53.1 SbCI,
20 $8.2
30 64.6
40 71.8
60 88.4
73 100
—47.8* O waCJIiCHa
— 49t 6.9 " +1.1
—40 12.3 1.1
—30 20. 1 "
— 20 31 "
— I4t 40 z.i+SbOi
o 46.1 SbOa
zo 51.6
20 57-4
40 72.8
60 89. z
73 100
Gms. SbCI| CqIii]
6.2^ o ^aCACH^
3 12.7
o 23.5
• 3 32.2
• 7St 43.8 "+sba.
o 47 . 2 SbCU
zo 52.2 "
30 64.8
40 72.3 "
so 80.2 "
60 88.8
70 97.4
SbGs + 0 Nitrotoluene. SbGa + m Nitrotoluene.
f .S^^r^^ Solid
r. per xoo urns. pKa-p
Sat. Sol. ,^°^^
« (Gms. SbGa
t*. per xoc Gms.
Sat. SoL
SoUd
Phase.
- 8.S* O
-13. S "-3
-i8.st 18. s
—10 2Z.3
+10 3Z.X
20 39
30 SO
34.5*62.3
33 68
27. st 74.6
40 79-1
50 84. 5
70 975
tfNOiCACHt
*(
I.I
ti
«<
M
•(
+1.1
z6*
zo
o
— xo
— 20
o
IS
30.7
39-2
42.8
crystallization not
obtained here
"+Sba
SbCW
o
20
30
40
SO
60
73
67.2
72. S
76.3
80.8
86
9X.6
100
SbCU + P Nitrotolaene.
Gns. SbCla c^itj
f . per xoo Gms. ^
Sat. SoL "^•
«iNQK:ACHi 52. S* o ^NOkCACHi
4S 18. 5
35 33.6
30 38.8
«• ao 46 -
75 t 52 - +1.1
7.5 62.3 i.i
SbOi s 66.x ••
3t 68. s 1.1+SbCa,
•• 10 70 SbO.
30 ^75. 5
SO 8s
70 97. S
l.I =
case.
2.1 =
Btituent.
* m. pt. t Eutec. T tr. pL
compound of equimolecular amounts of the two constituents in each
compound of 2 molecules of SbCk with i molecule ot the other con-
ANTIMONY TriCHLORZDE
94
REaPROCAL SOLUBILITIBS OP ANTIMONY TrICHLORIDB AND VARIOUS OrGANTC
Compounds, Dbtermined by thb "Synthbtic Method."
(MenKhutkin, iQio.)
SbCU + 0 Xylene.
SbCU + m Xylene.
SbCU + p Xylene.
Cms. SbCU
t*. per loo Cms.
Sat. Sol.
Solid
Phase.
Gnu. SbCU
t*. per 100 Cms.
Sat.SoL
Solid
Phase.
Gm^. SbCU
t*. per 100 Gms.
Sat.SoL
Solid
Phase. ^
— 29. 0 0
Ca(CH,)f
"57*
0 m C«H4(CHa)fl
14*
0
^CA(CHOt
-35 1 14
" +1.
x-60.5
t 7.S
" +I.X
II. 7
tii.7
" +X.I
-30 17. 5
X.I
-45
15.8
x.x
20
17. S
x.x
— 20 24.8
If
-25
29
ft
40
37.3
t«
-10 33.4
ft
- S^
46.2
ft
5®x
S2.3
M
0 43-4
f(
- 2t
49.8
" +a.i
sst
62.7
•• +a.x
10 55
M
5
53-1
9.1
60
66.1
a.x
19.5*68.1
l«
IS
S8-7
ff
7o*
81
«•
25 71 -3
a.i
25
657
ff
^5,
88.1
•<
30 75.7
i«
33^
73.8
N
S8t
92
" +sbcu
33.S'*8r
-. **
38*
81
(f
69
97.2
SbCU
3i.5t82.5
a.i+SbCl.
36.5
183.7 a.x+SbCU
a ■ •
• ■ •
• ■ • •
50 88
SbCU
SO
87.7
SbCU
10
20 . 7 ^ CACCHi)! unstable
60 92.4
f«
60
91. S
ff
7t
32.8
"^+a.x ••
71 98. S
70
97.2
ft
3S
55
SO. 3
62.7
a.x -
W M
• m.pL
t Eutec.
ttr.pt.
1. 1 = compoi
Lind of eqi
iiimoleci
liar amounts of the two constituents in each case.
2.1 » compound of 2 molecules of SbCU with i molecule of the other con-
stituent.
Distribution of Antimony Tri and Pbntachlorides between Aqueous
HCl AND Ether at Room Temperature
(Mylius, 19ZX ;
When I gm. of antimony as SbCU or as SbCU is dissolved in 100 oc. of aq.
HCl of the following strengths and the solution shaken with 100 cc. of ether,
an amount of metal, dependmg upon the concentration of the aq. add solution,
enters the ethereal layer.
With 1% SbCU Solution.
With 1% SbCU Solution.
Per cent Cone.
oiHa
Per cent of Total
Sb in Ether Layer.
Per cent Cone
of HCl.
Per cent of Total
Sb in Ether Layer.
20
6
20
81
IS
ID
13
22
IS
lb
32
6
S
I
8
0.3
S
I
2.5
trace
Solubility data determined by the freezing-^oint 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, diphenylmetnane and triphenylmethane (Kurnakov,
Krotkov and Oksman, 1915); SbBri, Sbli, and SbUri + Sbli (Bemadis, 1912);
SbCU (Aten, 1909).
ANTIMONY PentaCHLORZDE SbCU.
Data for the freezing-ix>ints of mixtures of antimony pentachloride and anti-
mony pentafluoride are given by Ruff (1909).
Gmft.
SbFa per
100 Gms.
Water.
Sat. Solution.
384.7
444.7
452.8
79.4
81.6
81.9
492.4
563.6
83.1
84.9
95 ANTIMONY TriTLUORIDB
ANTIMONT TrinUOaiDE SbF,.
Solubility in Water.
(RoKnheim and Grftnbaum, 1909.)
r.
o
20
22.5
25
30
Solubility ik Aqueous Solutions of Salts and of Hydrofluoric Acid at o^
Nonnality Gms. SbFs per xoo Gms. H^ present in Aq. Solutions of:
of Aq, Sah f ^ \
Solutioo. KG. KBr. KNQ,. KaS0«. EtC|04. (NH4)iQ04. KtC«H«0b. HF.
'l 461.8 448.7 458.2 419.9 465.7 ••• 461.4 432.5
0.5 448.3 450 451.9 408.5 481.2 431.9 430.5 404
025 431.9 455-6 418.3 406.6 451.3 442.3 430.8
o 125 407 -3 417-2 401.4 ... 405.2 433.3 435.2 *479.4
• (a » HF.)
Celluloid flasks were used and all measuring apparatus provided with HF re-
sistant coating. The SbFt was prepared in the form of rhombic transparent
crystals from SbA and HF.
ANTIMONT TrilODIDE Sbls.
S(x«uBiLiTY IN Methylene Iodide at i2^
(Retgers, 1893.)
100 parts CHsIt dissolve 11.3 parts Sblt. Sp. Gr. of solution » 3.453.
Solubility Data Determined by the Freezing-point Method Are Given
FOR Mixtures op:
Antimony triiodide and arsenic triiodide.
(Querdgb, 1912; Jaeger and Domboscfa, 1913; Vasilev, 19x3.)
" " " phosphorus triiodide. (Jaeger and Doraboech, 19x2.)
" " " iodine. (Querdgh, 19x2.)
AITTIMONY TriOXIDE Sb>Q|.
Freezing-point data are given for mixtures of antimony trioxide and antimony
trisulfide. (Querdgh, X9X3.)
ANTIMONY TriPHENYL Sb(C«Hi),.
Freezing-point data are given for mixtures of antimony triphenyl and mercury
dif^enyl and for antimony triphenyl and tin tetraphenyl. (Cambi. 191a.)
ANTIMONY SELENIDES SbSe, SbtSe.
Freezing-point data for SbSe + AgsSe and SbiSe -|- AgSe. (FOabon, X908.)
ANTIMONY TriSULPHIDE SbiS,.
1000 cc. water dissolve 0.00175 gm. SbiSt at i8^ (Weigd, X907.)
Solubility Data Determined by the Freezing-foint Method Are Given
for Mixtures of:
Antimony trisulphide and cuprous sulfide. (Panavano and Cesaris, 19x3.)
" ** " stannous sulfide.
^ " " lead sulfide. (Jaeger and Van Klooster, X9X3; P^bon, 19x3.)
M " '' silver sulfide. (Jaeger and Van Klooster.x9X3,)
ANTIMONY TARTRATE
96
ANTIMONT Potassium TARTRATE C2Hs(OH)s(COOK)(CXX)SbO).iHA
100 ems. water dissolve 5.9 gms. salt at room temp.
.? " " 6.9 " " " 25^
95% HCOOH dissolve 82.7 gms. salt at 20.8^
glycerol dissolve 5.5 gms. salt at 15.5*^.
II
(Squire and Caines. 1905.)
(S and S, 1903.)
(Aschaa. i9X3«)
(Aschan, 19x3.)
Solubility of Antimony Potassium Tartrate in Aq. Alcohol
Solutions at 25**.
(Seidell, 19x0.)
Wt. Per cent
CiILOHin
Sofvent.
O
5
ID
20
30
Sat. Sol.
1.052
1.025
1.007
0.980
0.958
Gms. C^IIA-
KSbO.mO per
xoo Gms. Sat. Sol
SSO
392
1.92
0.84
Wt. Per cent
C^mOHin
Solvent.
40
50
60
70
100
Sat. Sol.
0-93S
0.913
0.890
0.866
0.788
Gms-CiHA-
KSbO.iHiOper
100 Gms. SiO. SoL
0.38
0.23
0.12
0.06
trace
ANTIPYRINE CuHisN,0.
100 gms. water dissolve 80 gms.CuHuN20at 15^ (Greenish and Smith. '03.)
«4
II
II
II
II
II
«l
alcohol
90% alcohol
chloroform
ether
pyridine
50% aq. pyridine "
100
ICO
75.2
100
1-3
38.0
79.61
41
II
II
II
II
II
II
il
II
II
II
II
II
II
II
II
II
at 20-25'
II
(U.S. P.)
(EneQ. 1899.)
(Dehn; 19x7.)
The Solidification Points of Mixtures of Antipyrinb and Chloral
Hydrate.
(Tsakalatos, X9X3.)
|. ^j Gms. CuHnN^
rof Gms. CiiHttNiO g^j-j
Solidification. ^^Si^' P»««^-
108.9 100
90 86.1
70 73
5o.5Eutec. 64.2
60 56.8
62.3m.pt. 53.2
60 50.3
56 Eutec. 47 . 2
CuHmNiO
il
II
"+X.I
x.x
i<
II
<f
+i.a
Solidification.
60
61.8 m. pt.
57
SO
40
33.8 Eutec.
40
51.6
per xoo Gms.
Mixture.
40.9
36.7
30- 1
26.1
20.2
16.5
6
o
SoUd
Phase.
x.a
a
II
x.a+C(n,.C0H.Hi0
CCU.C0H.H/>
i<
i.i =» CiiHiiNiO.CCUCOH.HiO (Hypnal).
1.2 - CuHiiN,0.2(CCU.COH.H20) (Bihypnal).
The Solidification Points (Solubility, see footnote, p. i), of Mixtures of
' Antipyrinb and Salol.
(Bellucd, 19x2, X9X3.)
Initial r of
Solidification.
112. 6
104.5
98
91
83
7S
Gms. CuHitN^
per xoo Gms.
Mixture.
100
90
80
70
60
SO
Initial t*of
Solidification.
65
S3
30 Eutec.
34
3S
42
Gms. CuHisN^
per xoo Gms. <
Mixture.
40
30
17
20
10
O
97 APOMORPHZNB HTDBOCHLORIDS
APOMOBPHZNS HTDBOCHLORIDE CnHnNOk.HCl.
100 gms. water dissolve 1.7 gms. salt at 15^ and 2 gins, at 25^
100' gms. 90% alcohol dissolve 2 gms. salt at 25^
(Dott, Z906; Squires and Gaines, 1905.)
ABACHIDIC ACID C^HtoOi.
Sqlubilitt Data Determinbd by thb Frebzing-foint Method are
Given bt Meybr« Brod and Soyka (1913), for Mixtures of:
Arachidic and Stearic Acids.
" Palmitic Adds.
" " Lignoceric Adds.
ABBUTIN CuHisOr.iHsO.
100 gms. trichlorethylene dissolve o.oii gm. arbutin at 15^
(Wester and Bruins, 1914.)
ABGON.A.
Solubility in
Water.
(Estrdcher— Z. phjmk. Cfaem. azv xa4f W) %
^« Cor. Bar.
Vol. Vol. Absorbed
Absorption Coefficients.*
Soliibilitjr.
«.
/. *
V
0 • • •
... ...
...
00578
0.0102
I 764.9
77.40 4.34
0.0561
0.0561
0.0099
5 7650
77-39 3-93
0.0507
0.0508
0.0090
10 765-3
77-41 3.49
0.0450
0.04S3
0.0079
15 762.4
77 46 3-13
0.0404
0.0410
0.0072
20 7S7-6
77-53 2-86
0.0369
0.0379
0.0066
25 766.7
77.62 2.64
0-0339
0.0347
0.0060
30 760.6
77-73 2-43
0.0312
0.0326
0.0056
35 757 I
77.86 2.24
0.0288
0.0305
0.0052
40 7583
77.99 2.07
0 -0265
0.0286
0.0048
45 756.4
78.15 1.92
0.0246
0.0273
0.0045
50 747.6
7831 1-73
0.0221
0.0257
0.0041
a ^tinder barometric pressure minus tension of H,0 vapor.
/ —under 760 mm. pressure.
q —grams argon per zoo g.H,0 when total pressure is equal to
> 760 mm*
* See Acetylene,
pagez6.
SoLUBiLrrY OF Argon and Water.
(von Antiopoff, 1909-10.)
t". Coef. of Abs(»ption.
o 0.0561
10 0.0438
20 0.0379
30 0.0348
40 0.0338
50 0.0343
The ooef . 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 (191 7).
Data for the solubility and diffusion of aigon in solid and liquid metals aie
given by Sieverts and Bergner (1912).
ABSINIC 98
AB8ENIC As.
Data for the fusion-points of mixtures of arsenic and iodine are given by
Jaeger and Doomboech (1912).
MetaASSINIC ACID AsOiH.
Distribution at 25^ between:
(AueriMch, 1903.)
HsO and Amyl Alcohol. Sat. Aq. H|BOi Solution and Amyl AlcohoL
Gms. AaOkH per 1000 oc Gms. AaO|H pet 1000 oc
\q. Layer.
Alcoholic Layer.
Aq. Layer.
Akoholic Layer.
4.82
0.90
9.28
1-75
963
I -75
18.74
3-47
18.44
350
AB8INIC TriBBOBODE and TrilODZDE AsBr, and Asl<.
100 gms. H|0 dissolve about 6 gms. Asit at 25**. (U. S. P.)
100 gms. carbon disulfide dissolved about 5.2 gms. Aslt. (SquixesO
ICO gms. methylene iodide, CHtItt dissolve 17.4 gms. Asl| at I2% d of sat
solution » 3.449. (Retgers. 1893.)
Solubility Data EfETERMiNED bt the Freezing-point Method Are Givbn
FOR Mixtures of:
Arsenic tribromide and naphthalene. (Pushin and Kriger, 19x4.)
" " " phosphorus triiodide. (J^ser and Doombosch, Z9Z3.)
" triiodide and iodine. ■ (Qucrdgh, x9za.)
AB8ENIC TriCHLOaiDE AsCU.
When i.o gxn, of arsenic as the trichloride is dissolved in 100 cc. of aq. HCl
and the solution shaken with 100 cc. of ether the following percentages of the
metal enter the ethereal layer; with 20% HCl, 68%; 15% HCl, 37%; 10%
HCl, 7%; 5% HCl, 0.7% and with 1% HCl, 0.2% of the arsenic (MyUus. xgix.)
ABBSHIO TBIOXIDK As,0..
Solubility op the:
Crystallized Modification. Amorphous Modification.
In Water. In Water.
Ao Gms. AasOfe per
• • xooccHiO.
ord. temp. 3.7
b. pt. 11.86
In Alcohol, Ether and CS,.
G. AaiOs per zoo g. Solvent.
Alcohol 0.446
(Bniner and St. ToUoczko — Z. anarg. Chem. 37, 456, Ether o . 454
'o3;Chodouiiaky — Lucy. Chezn. 13, ZX4, '88.) pc ^ ,^,
(Widder — J. pr. Chem. [a] 31, 347, *85.)
SoLUBiLmr OF Arsenic Trioxtoe in Aqueous Solutions of Ammonia at
30*^ (Interpolated from Original Results).
(Schiememakers and deBaat, X9X5.)
Gms. per xoo Gms. Sat Sd. _ ... _. Gms. per xoo Gms. Sat. Sol.
*•.
Gms. AssOfe
per xoo cc.
Sat. Solutiaii.
2
1. 201
IS
as
1-657
2.038
39-8
b. pt
2.930
6.+
NH..
AsA.
■k ooua irnaae.
NH..
AsA-
-^ doiia roase.
0
2.3
AsA
4
7.6
NH*AsO,
I
8.3
u
5
6.2
2
14.9
«
7
4.6
2.8
20.5
AsA+NH4AsOi
10
31
3
13
NHtAsO*
13
2.4
3.5
9.1
«
14.3
2.2
99
ARSENIC OXIDBS
Sqlubilitt op Arsbnic Trioxtob in Watbr and inT. Aqueous Solution
GP Hydrochloric Acid at 15"* (Interpolated from the original).
(Wood, 1908.)
Mob. Helper
Liter.
O
0.46
2
4
Cms. Afl^jxr
zoo cc. SmuUoii.
1-495
1-5
1.2.
»-3
Hob. Ha pet
Liter.
6
7
8
Cms. As^per
100 cc Solutioii.
3-8
7.5
12. S
17.7
SoLUBiUTT OP Arsenic Trioxidb in Aqueous Salt Solutions.
(SdudBemaken and deBaat, 1917.)
In Aq. Ammonium Bromide at 30^
Gnu. per loo Gms. Sat. Sol.
AsA.
2.26
2.25
0.679
0.518
0.386
0-303
0.237
O.IS4
0.190
o
NH«Br.
O
0.339
4.37
7.18
13-31
20.14
31.69
41 -34
45.66
44.8
Solid Pbaae.
AaA
"+A9AJ^H«Br
AsA.NH«Br
In Aq. Sodium Bromide at 30^
Gms. per 100 Gms. Sat. Sol.
M
M
U
"+NH«Br
im«Br
AsA.
2.19
2.09
1.88
1.63
1.50
1.20
0.953
0.852
0.719
o
NH«Br.
SS7
10.89
20.79
30.39
3S-7S
39 24
43 64
45-99
50.25
±49-5
Solid Phase.
AaA
u
w
(AflA)iNaBr
<f
M
" +NaBr.dH«0
NaBr.aH/)
In Aq. Barimn Bromide at 30^
Gms. per loo Gms. Sat. Sol.
AiA.
2.09
2.03
1.97
1.87
1.58
0.7S7
0.678
0.464
0.322
0.277
o
BaBr^
9.41
16.88
24.03
24.41
23 -49
29.09
33 08
38.19
43.02
50.03
50.62
SoUd Pbaae.
AaA
In Aq. Barium Chloride at 30^
Gma. per zoo Gms. Sat. SoL
u
«(
ff
(As^OtBaBi^
«<
u
*l
il
" +BaBrt.3H,0
BaBrt.2H|0
AaA.
2.24
2.20
2.19
2.15
1.69
1. 12
0.905
0.737
0.608
0.506
O
BaClt.
3.84
8.72
8.86
10.34
9-55
13.62
16.93
20.06
23 87
26.54
27.6
Solid Phase.
AsA
II
M
l<
(AaA)i'BaCli
II
II
II
i(
" +BaCl,.2Hi0
BaCl|.2Hs0/
In Aq. Caldum Bromide at 20^ In Aq. Calcium Chloride at 19.5^-20^.
Gms. per loo Gms. Sat. SoL
AsfO^
1.58
1.28
0.912
0.789
0.698
0.513
0.687
O
CaBrs.
9-65
20.13
34.90
41
47.67
52.06
58.22
58.20
Sdid Phase.
AsA
Gms. per zoo Gms. Sat. Sol.
II
+CABri.6B,0
CaBr9.6H^
AsA.
1.78
1-39
1. 01
0.865
0.757
0.697
0.675
o
Cadi.
O
12.66
23 09
27.68
31.85
36.01
41.92
42.7
Solid Phase.
AaA
II
i<
M
II
M
" +CaCU.6H,0
CaClt.6H|0
SCO gms. 95% formic add dissolve 0.02 gm. AssQi at 19.8^ (Aschan, X9Z3.)
AB8INIC OXIDBS
100
S(H.UBiLrrY OF AxsBNic Trioxidb in Aqueous Salt Solutions. {Continued,)
In Aq. Lithium Bromide at so**.
Gms. per xoo Gnu. Sat. SoL
AaA.
2.26
1.69
1.20
0-734
0.534
0332
0.281
0.198
o
LiBr.
O
11.68
23-23
35 54
37
42.62
43 87
46.75
59.62
Solid Phaae.
In Aq. Lithium Chloride at 30^
Gms. per xoo Gms. Sat. SoL
[Sdid
AsA
" +(AflA)sXiBr
(AsA)sXiBr
(I
M
LiBr.HdO
AaA.
1.69
115
0.77
0.54
0.43
0.39
0.38s
0.41
O
Lia.
7-57
15-30
22.67
29.04
35-37
41.13
43-01
45-12
46.1
AaA
M
M
M
M
M
UCLH^
In Aq. Potassium Bromide at 30°.
Gms. per xoo Gms. Sat. Sol. Solid
Phase.
In Aq. Potassium Iodide at 30''.
Gms. per xoo Gms. Sat. SoL
AsA+0
D
AsA Kfir.
2.25 0.336
0.818 2.51
0.460 12.78
0.327 22.59
0.290 27.40
0275 36.98
0.207 39 04
0.166 42.07 "+KBr
o ±41.3 ^B'
2? variesfrom (AsA)fKBrto (AssOOrCKBr)*. O
In Aq. Strontium Bromide at 30^
Gms. per xoo Gms. Sat. Sol.
Solid
Phase.
AsA
(AaA),ja.
u
u
M
M
M
AsA.
1.69
1-74
1.48
1-25
1.07
0.991
o
SrBrt.
11.69
22.09
31.98
41.91
46.87
48.91
49.11
SoUd Phase.
AsA
AsA. KL
2.26 O
0.772 I. 19
0.296 9.56
0.183 22.89
0.150 34-31
O.II9 40.79
0.081 47.07
o.iiS 53-51
0.134 60.54
61.5
In Aq. Strontium Chloride at 30^
Gms. per xoo Gms. Sat. Sol.
M
"+KI
KI
If
K
U
U
"+SrBr,.6Hi0
SrBrs.6Hs0
AsA-
2.14
1.92
1.67
1.46
1.28
1.23
O
SrCl,.
6.27
13.67
21.29
27-46
34 03
36.16
37-5
Solid Phase.
AsA
t(
M
U
M
" +SrC3|.6HdO
Sra,.6HiO
ARSENIC PENTOXIDE AssOi.
Solubility in Water.
(Menzies and Potter, 19x2.)
f.
— 10
O
+ 10
20
29.5
40
60
80
100
120
140
f.
Gms. AsA per
xoo Gms. Sat. SoL
SoUd Phase.
- 5
10.6
Ice
— 10
15-6
u
— 20
21.3
M
-30
25-1
M
-40
27.8
M
-50
29.9
«(
S'Si^t.^L Solid Ph.«.
36 . 2 AsA4HiO
xoo
Ioe+AsA4H^
AsA4HiO
— 59Eutec. 31.7
-50 32.6
-40 33-5
-30 34-4
-20 35.4
100 gms. 95% HCOOH dissolve 7.6 gms. AsiOs at I9^
<«
ti
CI
37-3
38.3
39-7
41.4
41.6
42.2
42.9
43-4
43-7
44-5
u
M
"+3AsA.SH^
3AsA.5H^
«f
M
(Aschan, 1913.)
lOI
AB8INIOUS SULFIDB
JUUXHIOUB SULFIDE AsiSi.
looo cc water dissolve 0.000517 gm. AaA at 18^. (Wdgd, 1907.)
Data for the fusion-points of mixtures of arsenious sulfide and silver sulfide
are given by Jaeger and Van Klooster (1912).
ASPABAaniE C4H8NA.H10.
SOLUBILITT /S-Z-ASPARAGINB, C4H8NiOl.HfO» AND OP i84-AsPARAGimC AciD,
C4H7NO4, m Watbr.
(Bmder — Z. physik. Chem. 47t 6x3, '04.)
^4-Aspangiiie.
/94-Aapinngfnic Add.
Gms.
Gms.
'^
Gms.
Gms.
t\ CAN«0»HsO t'.
CJIaNsOs-HbO
f.
C4H7NO4 t».
CHtNO*
perxoog.
ptf xoog.
per xoog.
per xoog.
HiO.
HsO.
HsO.
HaO.
0.7 0.9546 SS'S
10.650
0.2
0.2674 51.0
1.2746
7.9 1.4260 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.I7IO 98.0
5»-475
315
0.7514 80.5
3.2106
41 -4 5-6500
40.0
0.9258 97.4
5-3746
> cms. H^ dissolve 24
gms. asparag
Ine at 20*-25*.
(Dehn, 19x7.)
100 gms. pyridine dissolve 0.03 gm. asparag^ine at 20^-25^. **
.100 gms. ^% aq. pyridine dissdve 0.15 gm. asparagine at 20^-25^ "
100 gms. tnchlorethylene dissolve o.oi 8 gm. asparagine at 1 5^. (Wester ft Bruins, 19x4)
Data for the solubility of asparaginic acid in aqueous salt solutions are given
by WuTgler (1914).
ASPIRIN (Acetyl salicylic add) C<H4(0CH|C0)C00H.
100 gms. water dissolve 0.25 gm. aspirin at room temperature. (Squire and Gaines, 1905.)
100 cc. 90% alcohol dissolve 20 gm. aspirin at room temperature. '* "
ATBOPDIE CnHsNQ,.
Solubility of Atropine, CnHnNOt, and of Atropine Sulfate,
4 (CnH»NOi)s.SOi(OH)st in Water and Other Solvents.
(U. S. p.; MiUkr, 1903.)
Grams Atropine per ,00 Gmns. ^^^^^
Gmms Solvent.
Solvent.
f.
Solutioa.
Water 25
Water 80
Alcohol 25
Alcohol 60
Ether 25
Chloroform 25
Benzene 20
Carbon Tetrachloride 20
Ethyl Acetate 20
Petroleum Ether 20
Glycerol 15
AmUne 20
Diethylamine 20
P)rridme 20
Piperidine 20
50% Aq. Glycerol )
+ 3%H,BQ, )
Oil of Sesame 20
2
68
3
o
3
o
782 (20^)
21 (20^)
03 (20^)
99
661
88
83
Solvent. (U. S. P.)
0.222 (0.13*)
IIS
68.44
III. II
6.02
64.10
• • •
1. 1361(1.76 J)
3
34§
67f
73i
ii4§
(U. s. p.)
263.1
454.5
27
52.6
0.047
0.161
33
loir
0.25*
*Zalai»i9io. tAti7*,Sdiiiidel]DeiMr,i9oi. t(jad,z9X3. S SchoUs, 19x3. YBaxoniandBorli]ietto,x9zz.
▲TBOPINK
102
Distribution of Atropine between Water and Chloroform at 35*
(Seidell, 19x00.)
Gmft. Atrc^ne Added
per IS cc. HjO+is cc
CHCU.
Aqueous
Chlorofomi
b
Layer (a).
Layer (6).
a
o.oos
O.OOIO
0.0057
5-7
0.025
0.0021
0.0256
13.3
0.125
0.0049
0.1246
25 -4
0.625
0.0160
0.6267
39- 1
▲TBOPINK METHTLBBOBODE Ci7HiiN0k.CH,Br.
100 gms. water dissolve 100 gms. of the salt at room temp. (Squires and Calnes, 1905.)
1 00 cc. 90% alcohol dissolve i o gms. of the salt at room temp. " **
AZELAIC ACm CtHmCCOOH),.
Solubility in Water.
(Lamouxxmx, 1899.)
t®. = o 15 20
Gms. CtHmCCOOH),
per 100 cc. solution = o.io 0.15 0.24
35
SO
6S
0.45 0.82 2 20
ICO gms. 95% HCOOH dissolve 3.79 gms. azelaic acid at I9.4^ (Aschaii, 19x3.)
Distribution of Azelaic Acid between Water and Ether at 25^
(Chandler, 1908.)
Gms. C7Hu(C(X)H)t per 1000 cc.
Gms. C7HM(CCX)H)t per zooo cc.
Aq. Layer.
0.06
Ether Layen
0.47
1. 10
2.71
4.26
Aq. Layer.
0.40
0.50
0.58
Ether Layer.
s 83
7.40
8.6s
0.10
0.20
0.30
AZOBENZENE CeHt.N8.CeHt.
Solubility of Azobenzene in Several Binary Mixtures.
(Timmermans, 1907.)
Solvent, Binary Mixture of:
34.9% Butyric Acid + 65.1% HjO (= sat. sol.
at 2.3**)
36% Triethylamine + 64% HaO (= sat. sol. at
19.0
36.5% Phenol + 63.5% H3O (= sat. sol. at
65.30
71.4% Phenol + 28.
20.6**)
H2O (= sat. sol. at
46% Succinic Nitrile+ 54% H^O ( = sat. sol. at 54'') 56 . 9
t*
Gms. (OHiN)i per
w .
iooGniA.Sat.:SoL
6.4
0.46
10
0.55
20
I 13
30
1.92
40.6
2.9s
8.8
3.22
II
2.57
14
1.66
17.4
0.54
69.3
0.43
72.7
0.47
80
1.47
90
2.43
100
3. 45
23 -9
0.52
25.2
0.87
40
4. 45
60
10.3s
72.6
133 40
56.9
0.54
103
AZOBBNZENE
Solubility of Azobenzenb in Several Alcohols.
(Timofeiew, 1894.)
Gms. (Cai,N)s
Gms. (CiHtN)s
Sohent.
f.
per zoo Gms. , Solvent.
Sat.SoL '
f.
per 100 Gms.
Sat. Sol.
Methyl Alcohol
95
3.8 Ethyl Alcohol
10.5
5-88
a «
10.5
3 . 95 Propyl Alcohol
95
S-42
Ethyl Alcohol
95
5. 29
10.5
6.02
SoLUBiLmr OF Azobbnzexbs in Water and in Pyridine.
_ (Dehn, 1917.)
Solvent.
f.
Gms. Each Compound (Determined Separately) per
100 Gms. Solvent:
Asobenzene.
Diaxoanuno-
Dunethylamino-
bcniene.
axobenzene.
0.03
0.05
0.016
76.44
136.7
27.90
16.78
67.7
4. SI
Water 20-25
Pyridine 20-25
Aq. 50% Pjrridine 20-25
HydroxyAZOBENZENE C6H».N:N.C«H40H.
1000 CO. sat. solution in HtO contain 0.0225 em. CsHsN: N.CsH40H at 25^
1000 cc sat. solution in HiO sat. with CeHe contain 0.0284 gm. C6HiN:N.
C«H40H at 25^
1000 cc. sat. solution in CcHe sat. with HsO contain 15.20 gms. CcHfNiN.
CsH40H at 25®. (Farmer, igoi.)
Distribution results for hydroxyazobenzene between benzene and water gave:
cone, in C«H6 -s- cone, in HjO — 539 at 25®. (Farmer, 1901.)
AminoAZOBENZXNX C6HtN:N.CeH4.NHs.
Distribution results for amino azobenzene between benzene and water gave:
cone, in C^He -r cone, in HjO = 3,173 at 25**. (Farmer and Warth, 1904.)
AZOANISOL, AZOBENZENE, AZOPHENETOL, etc.
Solubility .Data, Determined by the Freezing-point Method (see footnote,
p. i), ARE Given for the Following Mixtures:
^ Azoanisol
+ p Azoxyanisol (i)
+ p Azoanisolphenetol (i)
+ Methylpropylazophenol (i)
4- P Azopnenetol (i)
P Azoxyanisol
+ P Azoanisolphenetol (i)
+ ^Azoxyphenetol (3), (4)
+ Benzene (2)
+ Ethylene bromide (2)
+ Hydroquinone (5)
+ Benzophenone (5) ^
+ P Metnoxycinnamic Acid (5)
-|- Nitrobenzene (2)
p Azoanisolphenetol
^ +Azophenetol (i)
" -i-p Dipropylazophenetol (i)
Azobenzene
+ Azoxybenzene (6)
-f p Azotoluene (7)
+ p Azonaphthalene (7)
+ nenzalaniline (7)
P Azobenzoic Acid Ethyl Ester
' -{-p Azoxybenzoic Acid Ethyl
Ester (5)
(I
It
ti
II
II
II
II
If
II
II
II
If
11
II
II
II
11
II
II
II
If
Azobenzene
+ Benzeneazonapthalene (9)
+ Benzil (8)
+ Benzoin (8)
+ Benzylaniline (7), (9), (10),
(11), (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)
** +p Dipropylazophenetol (i)
p Azoxyphenetol
+ Cholesterylisobutyrate U)
+ Cholesterylpropionate (4)
-j- Cholesterylbenzoate (4)
+ p Methoxycinnamate (4)
P Azotoluene
+ Stilbene (7)
II
II
II
(7) rascal and Normand, 1913; {.H) vanstone. 10x3; (9) iseck, 1904; (10) Isaac (1910-1 z);
1907; (13) Hasaelblatt, 1913; (13) Garelli and C^alzolan, 1899; (14) Bruni and (jomi, 1899.
Azounmns
104
(Dehn, 1917.)
AZOLITMINE CTH7NO4.
100 gms. HsO dissolve 39.5 gms. azolitmine at 20^-25**.
100 gms. pyridine dissolve 0.05 gm. azolitmine at 20-25^.
100 gms. aq. 50% pyridine dissolve 0.12 gm. azolitmine at 20*'-25^. ^
AZOPHENETOL {p) CJl5N,.C,H«.0C,H,
Solubility in 100 per cent Acetic Acid.
(Dxeyer and RotaxBki — Chem. Centr. y6, U, xoi6, '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 /9 modification.
BARIUM ACETATE Ba(CH,COO)s. .
Solubility in Water.
(Walker and Fyffe, 1903; Krasnicki, 1887, gives inoinecflTesults.)
Gms. Ba(CHsCOO)i Cms. Ba(CHsCOO)i
t». perxoeGms. Solid Phase. t*. per 100 Gma. SoKd Phase.
Water. Solution.
40.5 79.0 44 I Ba(C,H,0,),
41.5 787 440
44S 77-9 43-8
51.8 76.5 43.4
63.0 74.6 42.7
730 73 S 42.4
84.0 74.0 42.5
99.2 74.8 42.8
Water.
Solution.
0.3
58.8
37 0
7-9
6i.6
38.1
17s
69.2
40.9
21 .6
72.8
42.1
24.1
78.1
43-9
26.2
76.4
43-3
30.6
75-1
42.9
35 0
75-8
431
39-6
77-9
43-8
Ba(C^O,),.3H,0
ti
t(
It
«
Ba(C^O,),.I^O
«
It
Transition temperatures 24.7° and 41°.
.100 cc. 97% ethyl alcohol dissolve 0.0723 gm. barium acetate at room temp.
(Crowell, 19x8.)
S(x.uBiLiTY OF Barium Acetate in Aqueous Solutions of Acetic Acid
AT 25*.
(Iwaki, X9I4-)
Mols. per 100 Mols. Sat. Sol.
CHiCOOH.
(CHtCOO)fBa.
Solid Phase.
CHiCOOH.
7'J'.j:,^" SolidPhase.
(CHsCOO)tBa.
lO
S.18
(CHiCOO)2Ba.3H20
28.72
4.52 3-3-"
0.41
5-21
u
36.54
5.60 "
1.40
5-34
" +3.3."
42.08
7.85 ;;
1.46
5-32
3-3-"
46.51
8.87 " +1.3
3 30
348
a
51.98
8.62 1.3
10.23
314
tt
65.77
8.40
20.60
3.62
tt
85.27
7.36
3.3.1 1 =3(CH,COO),Ba.3CH,COOH.iiHA i.3 = (CH,COO),Ba.3CH«COOH.
BARIUM ARSENATE Ba.(As04)s.
100 gms. H,0 dissolve 0.055 gfm. Ba,(As04),; 100 gms. 5% NH4CI
dissolve 0.195 gm., and 100 gms. 10% NH4OH dissolve 0.003 S^-
Ba.CAsOJ,
(Field — J. Ch. Soc. zi 6. 1859.)
BARIUM BENZOATE (CeHtCOO),Ba.6HsO.
100 gms. sat. aqueous solution contain* 4.3 gms. salt (anhydrous ?)* at 15^
and 10. 1 gms. at lOO**. CTuugi and Checchi, igozO
I05
BARIUM BORATE
BARIUM BORATES.
Solubility in Aqueous Boric Acid Solutions at 30**.
(Sboigi, 1913.)
Cms, per loo Gins.Sat. Sol.
B^Ob. ' BaO.
3.6 0.04
3.4 0.04
• 2.5 0.04
2.0 0.04
i.o 0.05
0.5 0.09
0.4 0.12
1.3.7 = BaO.3BjO1.7HfO (Triborate); 1.1.4 = BaO.BsO»4HfO (Metaborate).
The original results were plotted and above figures read from curve.
Solid Phaae.
BatOi.
BaO.
-: Solid Phase.
H,BO,+ 1.3.7
0.3
0.23
1.3-7
1.3-7
0.3
0.31
I.37+I.I.4
0.2
0.8
1. 1.4
0.2
1.2
((
0.24
4.8
cc
0.26
5.8
i.i4+Ba(0H),
0.08
53
Ba(OH),
BARIUM BROICATE Ba(BrOk)iHiO.
Solubility in Water.
(Trant^and Aoachtttz, 1906; Rammelsberg, 1841.)
Cms. Ba<BrO|)a Gms. Ba(BrOa)s Cms. Ba(BrO])]
t*. per zoo Cms. t*. per zoo Gixis. t^. per zoo Cms.
Solntioa. Soludoa. Soiudaii.
— 0.034 0.28 30 0.9s 70 2.922
0 0.286 40 1. 31 80 S-S^i
■f-io 0.439 SO I 72 90 4.26
20 0.652 60 2.271 98.7 S'^S^
25 0.788 99.65 5.39
SoLUBiLiTy OF Barium Broicatb in Aqueous Solutions of Salts at 25^
(Harkins, igzz.)
Cooc of Salt Cms. Ba(BiOi)a Dissolved per Liter in Aqueous Sol. of:
IB onis. i^iuv'
alents per Liter.
0
0.025
0.050
O.IOO
0.200
' KNOi.
7.93 (1.0038)
8.62 ^1.0059)
9.91 (i.cx>8o)
10.25 (X.0I20>
* • •
Ba(NO»)i. KBiOi.
7.93 ^ ^ 7.93 ^
7.22 (1.0059) 5.216(1.0046)
6.83 (1.0083) 3.415(1-0062^
6.415^1.0132) 1.72 (1.OIO9)
6.230(1.0233)
Mg(NOi)t.
7 93
• • •
• • >
8.196(1.0114)
• • •
FiguFes in parentheses show densities of the sat. sols, at ^r*
4
BARIUM BROMIDE BaBr,.2H,0.
Solubility in Water.
(Kiemcrs— Pogg. Ann. 99, 47, '56; Etard — Ann. chim. phy8.[7]at 5401 '94.)
Gms. BaBri per too
Grams.
Gms. BaBrs jper zoo
Grams.
%•.
Water.
Solution.
t\
Water.
Solution.
(Kxemen.)
(Kremers.)
(Etard.)
(Kremers.)
(Kremers.)
(Etaid.)
—20
• • •
• « •
45-6
40
114
S3 -2
51 S
0
98
495
47 S
SO
118
54-1
525
10
lOI
50.2
48.5
60
123
SS-i
S3-5
20
104
51.0
49S
70
128
56.1
545
25
106
Si-4
50. 0
80
^35
57-4
5S-5
30
109
S^i
50.6
100
149
60.0
57-8
140
• • •
...
S9-4
Sp- Gr. of saturated solution at 19.5° — 1.7 10.
BARIUM BBOBODI io6
Data for the system Barium Bromide + Barium Oxide + HfO at 25^ are
given by Milikau (1916).
Solubility of Mixtures of Barium Bromide and Barium Iodide in Water
AT Different Temperatures.
(EUid.)
Gfams per 100 Gms. Somoon. ^ Grama per ico Gna. Soantkai.
BaBrs. Bats. BaBrj. Bal».
—16 4.8 58.4 170 II. o 67.4
h6o 5.5 66.0 aio 14.9 67.7
135 9.3 67 . 3 Both salts present in solid phase.
Solubility op Barium Bromide in Methyl and Ethyl Alcohols.
(de Bruyn — Z. pbynk. Chem. xo, 785, ,9a ; RicfaaidB — Z. anocg. C3iem. 3» 455, '93 ; RoUand — Ibid.
15 4X9, '97.)
Parti BaBrj per 100 Parts BaBr».jHsO_per xoo
A o parta Aq. CAOH of: parta of Aq. CH«OH'of :
» • / » s . -^ .
xoo%. 97%. 87%. xoo%. 93-5%. So%.
15.0 0.48 (BaBn-aHsO) 45.9 37.3 4.0
32.5 3 .. . 6 5^'^ * * * * * *
100 gms. sat. solution in methyl alcohol at the crit. temp, contain 0.4 gm.
BaBrt. , (Ceatnersswer, 19x0.)
Data for the lowering of the melting point of BaBrs by BaFs and by BaCU
are given by Ruff and Plato (1903).
BARIUM PerBBOMIDE BaBri.
^ Data for the formation of barium perbromide in aqueous solutions at 35^ are
given by Herz and Bulla (191 1). See reference calcium perbromide, p. 189.
BARIUM BUTTRATE Ba(C4H7Qi)t2HtO.
Solubility in Water.
(Deszathy — Monatih. Chem. X4* »40t *9S')
Gma. Ba(CJlTOs)9 per 100 Gms. . . Gma. Ba(C«Hr09)» per xoo Gma
Water. Solution. ' Water. SolutiQik.
o 37-42 37.34 so 36.44 36.77
10 36-65 36.83 60 37-68 37.36
30 36.13 36.55 70 39.58 38.36
30 3585 2638 80 42.13 29.64
40 35.83 36.37
100 gms. 97% ethyl alcohol dissolve 0.17 gm. barium butyrate at ord. temp.
(Crowell, X9x8.)
BARIUM CAMPHORATE BaCioHi404.4HiO.
Solubility of Barium Camphorate in Aqueous Solutions of Camphoric
Acid at i6**-i7*.
Qungfliach and Landrieu, X9X4.)
Gma. per xoo Gma. Sat. Sol. Gms. per xoo Gma. Sat. Sol.
^ Solid Pbaae.
M
U
X.3 + Ba Camphonte
BaCamphonte
l^ a Barium tetracamphorate; CioHu04Ba.3CioHic04.
Camphoric
Acid.
Barium
Camphonte.
Solid Phaae.
Camphoric
Acid.
Barium
Camphorate:
0.68
0.134
d Camphoric ac. + z.3
0.48
22.71
0.84
0.150
u
0.4s
32.19
0.693
0.20
x.3
0.50
37.22
0.38
2.59
u
0.51
40.99
0.44
II. 10
(1
0
42.59
107
BARIUM CAPBOATE
BABIUM CAPBOATE and BABIUM ISO CAPBOATE.
Solubility in Water.
(Kn&cli,
1893.)
(Kdnig,
1893.)
Barium Caproate (Methyls Pentan.)
B«(CHt.<%bCH(CHa)C^OO)s.
Barium lao Caproate (Methyl a Pmtan.)
Ba(CHaCHrCHa)CHsCH|COO)s.
Giiis.Ba(CcHnOi)s
■*
' GmB.Ba(C6H|iOs>a
!•.
per TOO
> Gms.
.Solid Phase.
per xoo
Gms.
.Soh'd Phase.
Water, i
Soludon.
Water.
Sdutidn.
O
II. 71
10.49
Ba(CH„Oa),^JH,0
14.34
12.54
BaCCH
[uOi)a.4H«0
lO
8.38
7-73
M
^3-33
11.77
M
20
6.89
6.45
M
12.67
II .26
M
30
5.87
5-55
M
12.37
II .01
M
40
5-79
5.47
M
12.42
11.05
M
50
6.63
6.21
M
12.83
11.38
M
60
8-39
7.74
M
13.63
11.99
M
70
11.09
9.98
M
14.68
12.80
«
80
14.71
12.82
M
16.24
13.97
«
90
19.28
16.16
M
17 -95
15 23
M
BARIUM CABBONATE BaCOs.
Solubility in Water.
(HoUeman, KoUrausch and Rose, 1893.)
Electrolytic conductivity method used.
1 liter HsO dissolves 0.016 gm. BaCQi at 8.8°, 0.022 gm. at 18**, and 0.024 ff^' ^^
24^*.
Solubility of Barium Carbonate in Water Containing CO^.
The average of several determinations at about 10°, by Bineau, Lassaigne,
Foucroyand Ber^^mann is i.io gms. BaCOa per liter water. Wagner (Z. ansd.
Zh. 6, 167, '67) gives 7.25 gms. BaCOi per liter of water saturated with CO2 at
4~6 atmospheres pressure.
Eleven determinations by McCoy and Smith (191 i)p of the solubility of
barium carbonate at 25° in water in contact with pressures of COs 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. = 4S.i i^s. HiCOt per liter and 0.028 mols. » 7.3 gms.
Ca(HCC)t)s per liter. The equilibrium constant is i^ » 2.24 X io~* and the
solubility product Ba X COi = fei = 8.1 X io-«.
Solubility of Barium Carbonate in Aqueous Solutions of Ammonium
Chloride at 30*.
(Kemot, d'A^ostino and Pellegrino, 1908.)
Gms.p(
T xooo cc. lUJ.
M.
Solid
BaCOi.
NHiQ.
Phase.
0.035
0
BaCOs
0.521
8.099
1.333
64.536
1.596
92.593
2
160.265
2.093
186.77s
2.256
268.920
Gms. per xooo cc. HjO.
Solid
BaCOi.
2.245
2.706
2.630
NH«a.
335.70
358.66
418.33
Phase.
BaCOs
NH4C1
2. 151
1.558
414.71
413.77
0.730
0
410.16
397.58
It
u
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 HtO" and in others ''Gms. per liter of solution." The saturation was
effected by adding just the necessaiy amount of one constituent to cause the
disappearance of the last particle of the other. The amounts so add^ were
determined by we^hing the flasks. At high concentrations of the two salts, the
sudden increase in solubility appears to indicate a molecular combination.
BABIUM CABBONATS
io8
Solubility of Barium Carbonate in Aqueous Solutions op Potassium
Chloride and of Sodium Chloride.
(Cantoni and Goguelia, 1905.)
In KClatB.pt. of Sol. In NaCl at B.pt. of Sol. Inio%KClSoI. Inio%NaClSol.
Gms. KCl
Gms. BaCOi
Gms. NaCl Gms. BaCOi
Gms. BaCOi
Gms.BaCX3i
per 100
Gms. Sol.
per xooocc
pa 100
Gms. Sol.
per xooooc
f.
per xooooc.
f.
per xooocc.
Sat. Sol.
Sat. Sol.
Sat. Sol.
Sat. Sol.
o.iS
0.0847
0.15
0.0587
10
0.2175
10
0.1085
1. 00
O.1781
I
0.0787
20
0.2408
20
O.II26
3
0.3667
3
0.1056
40
0.2972
40
O.I23X
10
0.4274
10
0.1575
60
0.3491
40
0.1303
30
0.5550
30
0.2784
80
0.4049
40
O.I4I8
Barium carbonate boiled with aqueous NH4CI is slowly but completely decom-
posed. The time required varies inversely as the concentration of the NH4CI
solution.
Data are also eiven for solubility in 10% aqueous KCl and NaCl at the boiling
point p the time factor being varied from i to 198 hours.
Data for lowering of the melting point of BaCOt by NatCOt are given by Sackur
(1911-12).
BABIUM CHLOBATB Ba(C10i),.lI,0.
Solubility in Water.
(Carbon, 19x0; Trautx and AnachUtz, 1906.)
AO
Sp.Gr. of
£t.SoL
I 195
Gms. Ba(C10a)i per xoo
XA
Sp. Gr. of
X.355
Gms. BaCClOOi per 100
It.
Gms.
Sat. Sol.
40
i*.
Gms. Sat. Sol.
0
20.3*
l6.9ot
35.8*
33i6t
XO
■ a •
24.3
21.23
60
1-433
42.6
40.05
30
X.274
28.2
25.26
80
1.508
48
45-90
25
• • •
30
27 -53
100
1.580
531
51-2
30
• • •
32
29 -43
105.
6 b.
pt.
Z.600
54.6
52.63
•C.
t (randil.)
The determinations of Trautz and AnschQtz 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.
BABIUM PerCHLOBATE Ba(C104)s.3H,0.
Solubility in Water.
(Carlson, xgxo.)
f.
o
20
40
60
Sp. Gr.
Sat SoL
Z.782
Z.912
3.009
3.070
Gms. BaCaOOt
per xoo Gms.
Sat Sol.
673
74.3
78.3
81
f.
80
100
120
140
Sp. Gr.
Sat. Sol.
2. 114
2.155
2.195
3.230
Gms. BaCCIOOs
per xoo Gms.
Sat. Sol.
83.3
84.9
86.6
88.3
BABIUM CHLOBIDE BaQs.aHsO.
Solubility in Water.
(Mulder. Engd, 1888; Etard, 1894.)
Gms. Badt per xoo Gms.
• .
Water.
Solution.
0
31.6
24
zo
33-3
25
30
35.7
26.3
25
37
27
30
38.2
27.7
40
40.7
28.9
50
43.6
304
f.
Water.
Solution.
60
46.4
313
70
49.4
33- 1
80
52.4
34.4
XOO
58.8
37
130
59.5
37.3
160
63.6
389
215
75.9
43X
Sp. Gr. of solution saturated at 0° = 1.25; at 20® = 1.27.
109
BARIUM CHLoami
SOLUBILITT OF MIXTURES OP BARIUM ChLORIDB AND AMMONIUM ChLOKIDB
IN Water.
At 30^. (Schreinemaken, 1908.)
Gum. per'ioo Gms. Sat. Sol.
At Varying Temps. (Schreinemakets, xgiob.)
Gms. per xoo Gms. Sat. Sol.
BaClt.
NH«C1.
Solid Phase.
f. -
BaCls.
NH4CI.
:- Solid Phase.
22. Z6
571
BaCIi.2EbO
16.2
8.07
16.10
BaCb.2ByO+NHta
18.36
ZO.06
(1
0
8.22
19.26
u
15-42
13.84
«
30
8.19
24.89
u
XO.89
20. ox
«
40
8.40
26.93
u
8.33
24.69
u
SO
8.55
29 -53
M
7.97
25.92
BaCli.2EbO+NHia
356
27.47
NHia
Solubility of Barium Chloridb in Aqubous Solutions of Barium
Hydroxide and Vice Versa at 30**.
(Schidnemakera, 1909-19x0, xgxob.)
Gms. per xoo Gms. Sat. SoL -. «j «t. Gms. per loo'Gms. Sat. Sol, «!..,».
BaCh.
BaO.
— * ooua rnase. <-
BaCb.
BaO.
-« ooua jrnase.
27.6
0
BaCIs.2HjO
Z8.67
4.61
Baa(OH).2EbO+Ba0.9H^
27.42
1.78
H
18.04
4.62
Ba0.9H^
J87.36
1.77
" +Baa(0H).2By0
17.08
4.60
u
'24.98
2.33
BaCl(OH).2EbO
12.81
4.58
M
21.46
327
t(
10.77
4.45
M
19.18
4.67
u
0
4.99
II
Solubility of Mixturbs of Barium Chloride and Barium Nitrate
IN Water:
At 30^. (Coppadoro» x9xa, x9X3-)
Gnis. perxoo Gms. Sat. SoL
BaCli.
6.06
13.75
16.14
22.70
26.11
26.64
26.91
27.38
Ba(NOk)t.
9.55
20
8
7
7
7
5
4
z
92
94
88
37
13
S8
Solid Phase.
Ba(N0«)s
M
M
II
Ba(N0i>t+BaCb.2Hi0
BaCb.2H^
II
II
At Varying Temps. (Etard, X894.)
Gms. per xoo Gms. Sat. Sol.
Solid Phase.
BaCb. Ba(N0i)t.
O 22.5 4.3 BaCb.2H«0+Ba(N0i)s
20 24.5 6
40 26.5 7.5
60 28.5 9.5
100 31 14
Z40 32 20
180 33 26 *•
210 32 32 "
II
u
u
u
a
Solubility of Barixtm Chloride in Aqueous Solutions op Copper
Chloride at 30** and Vice Versa.
(SchxciiiemakerB and de Baat, 1908-09.)
Ona. per xoo Gms. Sat SoL
Gms. per xoo Gms. Sat. Sol
BaCb.
CuCb."
ooua rnasB.
BaCb.
CuCb.
. OQua rnase.
0
43.95
CuCb.2H/)
5.49
30 76
BaCb.2H«0
1. 25
42.45
II
10.13
21.76
II
3.08
42.07
(misuble)
17.08
11.49
M
2.72
42.36
CaCb.2HiO +BaCb.2H«0
22.78
.5.13
II
2.84
41.18
BaCb.2HiO
27.6
0
M
398
37.42
II
Solubility data have been determined for the following systems:
BaCls.2H^ + Cuai.2HiO + NH4CI + HiO at 30®. (Schreinemaken, X909.)
+ " + KCl + HiO at 40** and 60*. ( " and de Baat. x9x4.)
+ " + NaCl + H|0 at 30**. ( " anddeBaat.x9o8-o9.)
+ BaO + NaiO -j- HtO at 30**. (Schreinemakers, x9xob.)
+ Ba(NOi)i + NaNOi + NaCl + HiO at 30'. (Coppadoro. X9X3.)
+ HCl + NaCl + H2O at 30''. CSchxeinemaken. Z909-XO. Z9xob0
«
it
ft
M
M
BABIUM CHLOBIDS no
Solubility of Barium Chloride in Aqueous Solutions of Hydro-
chloric Acid:
Ato*.
At 30".
(Engd, z888.)
(Masaon, igxz, 19x1-13; Schreinemaken. 1909-10.)
Sp. Gr.
Gms.perioo
HCl.
Gms. Sat. Sol.
BaCb.
Sp. Gr.
Sat. Sol.
Gms. per 100
Gms. Sat. Sol.
Sat. Sol.
HCl.
BaClt.
1.250
0
24.07
1.3056
0
27.84
1.242
0.32
23.31
I . 2651
1.36
24.02
1.228
0.83
22.11
I. 2147
3.32
19.20
1. 210
I-SX
20.14
1.1789
5. OX
15.2
1. 143
4.58
12.76
I . 1419
7.13
II. I
1. 118
6.13
9.37
I. 1068
10
5.8
1.099
755
6.33
1.0880
1343
2.4
1.079
10. 8z
2.64
1.0895
16.92
0.38
1.088
16.92
0.28
1 . 1024
20.62
0
I. 1609
32.18
0
The results of Schrememakers show that at 37.34% HCl the barium chloride
dihydrate is converted into monohydrate.
Less than i part of BaCls is soluble in 20,000 parts of concentrated HCl and in
120,000 parts of cone. HCl containing i volume of ether. (Mar, 1892.)
Solubility of Barium Chloride in Aqueous Solutions of Mercuric
Chloride:
Ato^
(Schrrinrmakers,
1910.)
At 30^
(Schieinemakers, 1910.)
Sms. per 100
Gms. Sat. Sol.
Solid Phase.
Gms. per zoo Gms. Sat. Sol.
Solid Phase.
HgCh.
BaCb.
HgCh.
BaClt.
0
23.70
BaOt-sHtO
0
27.77
BaClt.2H^
14.25
24
II
2.90
27.56
i(
36.20
24.89
II
12.98
26.99
M
46.08
24.05 Baat.3HgCli.6H«0+BaClt.2H<0
34.57
26.69
M
46.59
23.28
Baat.3HgClt.6HtO
46.50
25.22
<f
47.78
21.05
II
55."
23.17
" +Hgai
48.46
20.67
••+Hgat
48.97
17.87
HgOi
44.33
18.50
HgOt
41.30
14.26
If
29
"■59
If
27.62
8.41
w
16.36
6. II
II
14.19
2.65
«l
3. 95
0
<f
7.67
0
u
Solubility op Mixtures op Barium Chloride and Mercuric
Chloride in Water.
(Foote and Bristol — Am. Ch. J. 33, 348. '04.)
Gms. per xoo Gms. _ ...
*• Solution. Sohd
• ^r-z: * . ^. * Phase.
fiaCla. HgQs.
10.4 23.58 50.54 {^gjS:'^
XO.4 23.44 50.74 (Double Salt
10.4 22.58 51.23 jBaCi.3HgCI,.
10.4 22.48 51.41 ^ ^^"'
Gms. oer 100 Gms. . ^ „,
to Solution. ^SolM
6aa,. * HgCis. ^****-
10.4 22.10 51.66 {g^};!*3l5j*3^.,jH^,
10.4 21.64 Sl.74rB^ci...H.(H-H«CL.
35 23.02 54.83 1 ^^'"''^"•^
Solubility of Mixtures of Barium Chloride and
IN Water:
At 30^
(Schretnemakers and de Baat, 1908-09.)
Sodium Chi.oridb
At Varying Temps.
(Precht and Wittgen, i88z;
Radorff, 1885.)
Gms. Der 100 Gms. Gms. per
^..Sol. SoUd Phase. Sat.
too Gms.
.Sol. Solid Phase.
Gms. per xoo Gnu*
1*. Sat. Sol.
BaCb. Naa. BaClt.
0 26.47 NaO 12.25
2.28 25.28 " 15.83
3.80 23.77 " +Baat.2aO 20.93
5.76 20.25 Baai.2H<0 24.24
8.19 17.89 •• 27.60
NaCl.
13.39 Baai.2H^
10.06
5.39
2.76 "
0 "
BaClt. NaCL
20 2.9 25
40 4.5 23
60 6.8 23.4
80 9.4 22.8
XOO II. 8 22.2
Ill
BABIX7M CHLORIDE
SOLUBILITT OF MIXTURES OF BaRIUM ChLORIDB AND POTASSIUM ChlORIDB
IN Water. (Foote, 1904.)
100 gms. saturated solution contain 13.83 gms. BaCls + 18.97 gms. KCl at 25^
Fusion-point curves (solubility, see footnote, p. i) are given for the following
mixtures:
BaCl,-|-
+
+
+
+
+
+
+
+
+
u
tt
«l
•<
«l
«
«
14
l<
It
€1
«l
II
II
II
• I
fl
BaCO»
BaCi04
BaO
BaS04
BaFt
Bait
CdCli
CaCli
CuCU
PbClf
LiCl
MgCl,
MnCls
KCl
NaCl
NaCl+KCl
SrCl,
ZnCl,
TlCl
(Sackur, igzx-ia.)
«
(Sackur, X9xx-X2, Amdt, xQo?-)
(Sackur, 1911-13, Ruff and PUto, X903.)
(Botta. 191 x; Ruff and Plato, 1903; Plato, 1907.)
(Ruff and Plato, X903.)
(Sandonini, X9xx, 1914; Ruff and Plato, X903.)
(Sandonini, x9xx, 1914; Ruff and Plato, 1903; Schaefer, 19x4.)
(Sandonini, X9X4.)
(Sandonini, x9xz, X914; Ruff and Plato, X903.)
(Sandonini, x9X3, X9Z4.)
(Sandonini, x9za, X9X4.)
(Sandonini, 19x3, X9X4; Ruff and Plato, X903.)
(Sandonini, x9xi; Ruff and Plato, 1903; Vortiach, X9X4.)
(Sackur,x9xx-X2; Ruff and Plato, X903; Le(niatelier,x894; Vortitch, 19x4.)
(Vortisch, X9x4(a); (Semsky.)
(Sandonini, z9xx, 19x4; Ruff and Plato, X9Q3; Vortisch, X9X4.)
(Sandonini, X9X3 a, X9X4.)
(Korreng, X9X4.)
Solubility of Barium Chloride in Aqueous Ethyl Alcohol Solutions.
At I5^
At 30**. At 60**.
(Schiff. x86x;
Rohland, x897-)
(Schxeinemakers
and Mcasink, 19x0.)
ir^ or Gms-BaCb
3^§ per 100 Gms.
Gms. per
CsIbOH.
xooGms.
Sol.
BaCk.
SoUd Phase.
Gma.Der
xoo Gms.
Sol.
Solid Phase.
'"*^"- Solvmt.
CtHiOH.
Ba(ns.
10 31. I
0
27 95
BaCb.2H^
0
31.57
BaCh.2H^
20 21.9
32.67
10.63
16.68
20.16
30 14.7
50.16
5.68
34.10
13-21
40 10.3
60.72
2.23
66.02
2.82
60 3 5
92.53
0.05
88.55
0.25
80 0.5
94 73
0.06
" -f Ba(ni.HiO
90.25
0.09
" +Ba(n«.IW)
97 0.014
97.14
98.17
■ • •
0.08
Ba(1i.HiO
" +Bafnt
93.95
• ■ ■
BaCkHiO
»
99.41
■ ■ •
BaCli
100 gms. methyl alcohol dissolve 2.18 gms. BaCIs at 15.5° and 7.3 gms. BaClt.
2 HiO at 6**. (dc Bruyn, x89a.)
100 gms. glycerol dissolve 9.73 gms. BaCls at I5^-I6^ (Osaendowaki, X907.)
100 cc. anhydrous hydrazine dissolve 31 gms. BaCls at room temp.
(Welsh and Broderson, X9X5.)
100 gms. 95% formic acid dissolve 7.3 ^s. BaClj at 19 . (Aschan. x9X3.)
One Titer sat. sol. in nitrobenzene contains 0.167 S^' BaCls at 20^, 0.33 gm« at
50® and 0.40 gm. at 100**. (Lloyd, 19x8.)
Data for the system BaClt + Triethylamine + HjO are given by Timmermans
(1907).
Solubility of Mixtures of Barium Chloride and Glyqne in Water
AT 20*^. (Pfeiffer and Moddski, 191 3.)
Gms. per xoo cc. Sat. SoL
NBsCHs(X)OH. Bada.
5.5
26
37
16
Solid Phase.
BaC]i.2H^+BaCls.2NHiCHsC(X)H.H<0
NH4CHsC(X)H+Ba(ni.2NHsCHs(XX)H.H^
BARIUM CHBOHATE xi3
BARIUM CHROMATE BaCr04.
Solubility of Barium Chromatb in Water.
One liter of sat. solution contains 0.002 em. of the salt at o^; 0.0028 gm. at
10^; 0.0037 ^. at 20^ and 0.0046 gm. at 30 . (Kohlrauach. 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. BaCi04;
if ignited barium chromate is used, only 0.0062 gm. dissolves.
One liter sat. sol. containso.043 gm. of thesaltat boiling point. (Meachenaki, i88a.)
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 CHtC0tNH4 ana 0.022
gms. when the solvent is 0.5% sol. of NH4N0t.
One liter of 45% aq. ethyl alcohol solution dissolves 0.000022 gm. at room temp.
(Guerini, t9ia.)
BARIUM CnmAMATBS.
Solubility of Barium Cinnauates in Water, Methyl' Alcohol and Acetone.
Gmt. Anhy-
Compound. Fonnuk. t*. Solvent. p^^^Gm. Authority.
Sat. Sol.
Barium Cinnamate Ba(CiHiOi)i.3H<0 15 HtO 0.726 (Taragi and Cheochi,i9oz.)
«
« K
100
i«
2.27
M M
«
Allodnnamate Ba(CiH1(^^E«0
19
CE^H
15.8
(LieberiBaim,x903.)
u
a u
12
ti
IS. 4
(Michael and Garner, 1903.)
u
" Ba(aHiO«)^H<0
20
u
2.56
(Michael, 1901.)
u
« «
20
(CH^iCO
0.80
M
((
« 11
20
H^
6
M
M
Hydzodnnamate Ba(aHiOi)t.2HjO
27
i«
2.9
H
«
« «<
25
CHiOH
0.1
«(
M
« M
16
<i
9-7
(Michael and (jamer, 1SO13.)
M
Isocinnamate "
20
u
70
(Michael, 1901.)
M
<( w
20
(CHi)]CO
20
<i
M
« M
20
H^
17
M
BARIUM OITRATB Ba,(CeH«0,),.7H,0.
Solubility in Water and in Alcohol.
xoo grams water dissolve 0.0406 gram Ba,(C,H407)f.7HjO at 18®,
and 0.057a gm. at 25^.
zoo grams 95% alcohol dissolve 0.0044 gram Ba,(C«HsOT),.7HsO at
i8^ and 0.0058 gm. at 25^.
(Partheil and Hiiboer — ArduT. Pharm. 241, 4x3, 'qs«)
BARIUM OTANIDl Ba(CN),.
Solubility in Water and in Alcohol at i4*.
(Joannis — Ann. chim. phys. [5] a6^ 489^ *Sa^
100 parts water dissolve 80 parts Ba(CN)2.
100 parts 70% alcohol dissolve 18 parts Ba(CN)a.
BARIUM nRROOTAiriDB and BARIUM POTASSIUM FBRRO-
OYAHIDB.
(Wyrouboff — Ann. chim. phys. [4] z6^ 99a, '69.)
xoo parts water dissolve o.z part BaaFe(CN)«.6H,0 at Z5^ and z.o
part at 75**.
100 parts water dissolve 0.33 part BaK,Pe(CN)«.5H,0 at ord. temp.
BARIUM FLUORIDB BaFs.
Solubility in Water.
(Kohliausch, 1908.)
One liter sat. sol. contains 1.586 ems. of the salt at 10^; 1.597 gms. at 15^;
1.607 gms. at 20®; 1.614 gms. at 25 and 1.620 gms. at 30".
Freezing-point curves are given for mixtures of BaFs+KF by Puachin and
Baskow (1913), and for BaFt+Balt by Ruff and Plato (1903).
113
BABIUM FORMATS
BABIUM FORMATE Ba(HCOO)t. ~
S<X.UBILITY IN Water. (Staaky, Z904. See also Ensnicki. 1887.)
r. Gms. Ba(HCOO)i
per zoo Gms. Sat. SoL
r.
Gms. 6a(HC00)s
per zoo Gms. Sat. SoL
0
23 24
10
23.22
20
23 -^s
25
23 -9
30
24.2
40
25
so
25-9
60
26.9
80
29-3
100
32.8
Ba(OH)s.8HtO.
Solubility in Water. Solid Phase Ba(0H),.8H,0.
(Rooenthiel and Rfihlmanb— Jahztsber. Chem. 3x4* '70.)
o Gms. Ba(OH)i per zoo Gms.
"Water.
Sdutiaa.'
0
1.67
i.6s
5
I -95
i I 92
10
2.48
2.42
15
3 23
313
20
3 89
3-74
25
4.68
4-47
*•.
Gms. Ba(OH^
per zoo Gms.
Water.
Sdutka.
30
5 59
S-29
40
8.22
7.60
SO
13 12
II. 61
60
20.94
17 32
7S
63 SI
38.8s
3o
101.40
SO. 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)s.8HsO in HtO at 25''.
SoUd
Phase.
Sp. Gr.
Sat. SoL
Solubility of Barium Hydroxide in Aqueous Solutions of Barium
Nitrate at 25^ and Vice Versa. (Parsons and Carson, Z9ZO.)
Sp. Gr. Gms. per zoo Gms. HiO.
Sat' SoL Ba(OH)s. Ba(N0d«.
4.29 O Ba(0H)s.8H^ I-I37I
1. 1448
I.I2IO
I. 1002
1.0797
1.0512
I. 0651
1.0790
I -097s
I. 1220
4. 35
4.48
4.40
4.72
1.88
3-47
5.66
755
Gms. per zoo Gms. H«0.
Ba(0H)t.Ba(N0i)t.
4.93 I0.2I
u
u
u
tt
5 02
3-22
o
11.48
11.04
10.66
10.30
Solid
Phase.
BaCOHMHsO
" +Ba(NON)t
Ba(NO«)t
tt
M
Solubility of Barium Hydroxide in Aqueous Sc».utions of Alkali
Chlorides at 25^. (Hers, zgzo.)
In Lithium In Potassium In Rubtdium In Sodium
Chloride. Chloride. Chloride. Chloride.
Gnas. per zoo cc Sat. SoL Gms. per zoo cc. Sat. SoL Gms. per zoo oc. Sat. SoL Gms.perzooGc.Sat.SoL
■ IJCL
Ba(0H)«.
Ka. Ba(0H)a.
Rba.
Ba(0H)s: NaCL Ba(0H)s.
9-75
II
.45
25 -95 5-93
1511
5.55 16.
SI 6.91
6.02
8
•03
13 OS 5'^
0
4.76 8.
37 S-99
318
6
■39
8.60 S'53
...
4.27 S-40
0
4
.76
0 4.76
...
... 0
4.76
Solubility of Barium Hydroxide
IN Aqueous Solutions
of Sodium
• Hydroxide at 30**.
(Schreinema)
zeOt Z909-Z0.)
Gms. per zoo Gms. Sat. SoL
Solid Phase.
Gms. per
zoo Gms. Sat. SoL
Solid Phase.
BaO.
NasO.
BaO.
NsiO.
4.99
0
BaO.gOO
1.84
26.14
Ba0.4HiO
1.29
4.78
<i
1-75
27.72
If
0.89
6.43
M
1.58
^8.43
<i
0.57
9.63
II
1-34
29.24
" +Ba0.2HiO
0.53
11.62
M
0.82
32.12
Ba0.2Hi0
0.47
17.87
II
0.59
34.72
<i
1.06
23.28
M
0.57
41.09
" +NaOH.HiO
1.87
24.63
Ba0.9H^+Ba04HK) O
+42
NaOH.H40
BABIUM HTDBOZIDE
114
Solubility op Barium Hydroxidb in Aqueous Acetonb at 45®.
Sp. Gr.of
Solntiant.
yoi.%
Ba(0H)s per loo cc. Sat.
ScMUtion.
Gnu. Ba(0H)a
per
AcctaDC.
100 Gms.
Millimols.
Grams.
Solution.
1.0479
0
55 08
4.722
4.506
I .0168
10
31.84
2.730
2.686
09927
20
17 -79
I 525
1-536
0.9763
30
9.10
0.779
0.798
0.9561
40
4. 75
0.407
0.426
o.939«
SO
I 54
0.132
O.I4I
0.9179
60
048
0.041
0.04S
0.8956
70
0.08
0.007
0.018
t*.
Gms. Ba(IOa) pnr
zoo Gms. Soluaoa.
*•.
Cm. Ba(IQ{)t pa
too Gms. SoiudoflL
30
0031
70
0.093
40
0.041
80
o.iis
50
0.056
90
0.I4I
60
0.074
100
0.197
Data for the systems Ba(OH)i + Phenol + HiO at 25* and Ba(OH)i +
Resorcinol -f- H|0 at 30® are given by van Meurs (19 16).
BABIUM XODATE Ba(IO,),.HtO.
Solubility in Water.
CTrautz and Anschnte, 1906.)
«o Gms. Ba(IOB)2 per
xoo Gms. Solution.
— 0.046 0.008
+ 10 0.014
20 0.022
25 0.028
One liter sat. aqueous solution contains 0.3845 gm. Ba(IOt)t at 23^
(Harkins and Wmninghoff, 191 x.)
At room temperature Hill and Zink (1909), found 0.284 Z^* Ba(IO<)s per liter
sat. aqueous solution.
Solubility of Barium Iodate in Aqueous Salt Solutions at 25®.
(Harkins and Winninghoff, 191 1.)
Mob. Salt rSlwL\.
P" Liter. Bj^OO.
o.ioo 0.148
0.200 0.136
0.C02 0.396
o.oio 0.445
0.050 0.643
100 cc. cone, ammonia (Sp. Gr. 0.90) dissolve 0.0199 gm. Ba(IOs)t at room
temp. (Hill and Zink, 1909.)
100 cc. 95% ethyl alcohol dissolve o.ooii gm. Ba(IO0t at room temp.
(Hill andZink, 1909.)
BARIUM IODIDE Bal,.
Solubility in Water.
(Krenusrs — Pogg. Ann. Z03, 66. 1858; Etard — Ann. chim. phya. [7] a, 544, '94.)
Added
Salt.
Ba(N0>)i
Mols.Salt bSVSv
per Liter. Ba(IQO.
*t
o.oox
0.002
0.005
0.020
0.050
per Liter.
0.331
0.294
0.237
0.164
0.149
Added
Salt.
Ba(NOs)s
«i
KNOi
Added
Salt.
KNOi
KIOi
<t
«<
Mols. Salt
per Liter.
0.200
0.000106
0.000530
0.001061
Gms.
Ba(IOi)«
per Liter.
0.777
0.368
0.303
0.229
Gms. Bal2 ^r 100 Gms.
Water. ^
-20
O
+ 10
20
25
30
143 -9
170.2
185.7
203.1
2x2.5
219.6
Solution.
59 o
63.0
65.0
67.0
68.0
68.7
Solid Phase.
Gms. Bala 'pct 100 Gms.
Bal3.6 H3O
«
<(
((
40
60
80
100
120
160
231.9
247 -3
261.0
271.7
281.7
294.8
Solution.
69.8
71.2
72.3
73 I
73-8
74.6
Sdid Phase.
Bal,.2 H3O
<(
K
(I
l(
U
(Aschan, 1913.)
Sp. Gr. of sat. solution at 19^5 » 2.24.
100 gms. 95% HCOOH dissolve 75 gms. Balj at 20.2®.
100 gms. 97% ethyl alcohol dissolve 1.07 gms. Bal2.2HsO at 15". (Rohland, 1897.)
Data for the system Balt+BaO+HsO at 25° are given by Milikau (1916).
115
BABnJM PerXODIDE
BABIUM PerXODIDE Bal4.
Data for the formation of barium periodide in aqueous solutions at 25^ are
given by Herz and Bulla (191 1). (See reference calcium perbromide, p. 186.)
BABIUM rODOMEBCUBATE.
A saturated solution of Bait and Hgit in water at 23.5^ was found by Duboin
(1906J to have the composition BaIt.i.33HgIs.7.76HsO, a » 2.76.
BABIUM MALATE BaCH^O..
Solubility in Water.
(Cftntoni and Baaadonna — BuU.8oc.chiin.[3]35, 731, '06O
20
30
Gms.BaCiBLOs
per xoo cc. Sol.
*^
0.883
35
0.901
40
0.903
50
Gm8.BaC«ILOk
per xoo cc. Sol.
0.895
0.896
0.942
60
70
80
Gins.BaC«H|Ok
per xoo cc. SoL
I. Oil
1. 041
1.044
Solubility in Water and in Alcohol.
(fiarthcil and Hfibner — Archiv. Pharm. 241, 413* '03.)
ZOO grams water dissolve 1.24 gms. BaC^H^Os at 18^, and z.3631
gms. at 25^.
100 grams 95% alcohol dissolve 0.0038 gms. BaC4H405 at x8^, and
0.0039 gm. at 25**.
BABIUM MALONATE BaC,HsO4.2Hs0.
Solubility in Water.
(Micrynaki — Mooatah. Chem. 7$ 263, '86.)
*•.
Gms.BaCaHsO^
1 per xoo Gms.
f.
Gma.BaCsHaO^
perxooGi
Water.
Solutioa
Water.
Solution.
0
0.143
0.143
50
0.287
0.285
10
0.179
0.179
60
0.304
0303
20
0.212
0211
70
0.317
0316
30
0.241
0.240
80
0.326
0.325
40
0.266
0.265
Results slightly higher than the above, from 0^-50^ are given by Cantoni and
Diotalevi (1905).
BABIX7M MOLYBDATE BaMo04.
100 parts water dissolve 0.0058 part BaMo04 at 23^. (Smith and Biadbuxy, 1891.)
BABIUM HITBATE Ba(NO,),.
Solubility in Water.
(Mukfer; Gay Lusmc; Etaid — Ann. chim. phyB.[7] a, 528, 94; ^uler — Z. phytik. Chem. 40b 3X5t'o40
Gma.
Ba(N0k)a
Gma. Ba(NOB)s
f.
per
100 Gms.
t«.
per 100
Gms.
Water.
Solution.
Water.
Solution.
0
50
4.8
80
27.0
21.3
10
7.0
6.5
100
34-2
25 -5
20
9.2
8.4
120
42.0
29.6
25
10.4
9-4
140
50. 0
33-3
30
II. 6
10.6
160
58.0
36.7
40
14.2
12.4
180
67.0
40.1
50
17. 1
14.6
200
76.0
43-2
60
20.3
16.9
"5
84.5
45-8
Results from o*-35* differing from the above are given by Vogel (1903).
100 gms. sat. aqueous solution contains 4.74 gms. Ba(NOa)s at o^. (Coppadoio, 1911.)
BABIUM NITRATE
Ii6
Solubility of Mixtures of Barium Nitrate and Lead Nitrate in Water
AT 25^ (Fock, Z897; £uler, 1904.)
In Soltttiaii.
Sp. Gr. of
tian.
sp. i.
Gms. per Liter.
079
088
108
119
140
163
198
252
294
4^9
Ba(NOk)a.
102.2
549
86.5
79-7
77 o
69.8
66.0
575
25-9
28.8
Pb(NO|)s.
O
17-63
49.80
68.10
97.20
130.7
Mg. Mols^ per Liter.
Ba(NOt)a.
177
247
334
429
3
7
3
7
553 •«
391.0
210. 1
330.7
3049
294.4
266.8
252.5
222.6
99.2
no. 3
0.0
PlKNO,
o
53
150
205
293
395
535
748
loio
1298
1673
3
7
7
6
o
6
5
3
o
o
Mol.%
Ba(NCSs-
100
79.78
68.70
59-^
50.09
40.31
32.03
22.91
8. II
7-77
0.0
In Solid
Mol.%
B*(N(»i
100
98
96
94
93
92
90
83
75
35
o
30
74
80
62
49
07
47
44
II
o
Tables of results are also given for 15^, 30^ and 47'
S9LUBILITY0P Mixtures of Barium Nitrate and Potassium Nitrate in Water.
(Flndlay, Mocgan and Morris, 1914; Foote, 1904.)
r.
9.1
9.1
9.x
9.1
9.1
Gn». per xoo Gms. Sat. Sol.
21
21
21
21
2L
21
21
21
21
I
I
I
I
I
I
I
I
I
Ba(NOs)t.
6.2s
4.20
1.98
0.98
O
8.46
7-47
6.35
6.06
5. 98
3-35
2.30
1.76
o
a
KNO».
o
8. IS
12.02
16.80
16.76
o
2.12
5.98
8.47
13.24
18.24
21.47
24.86
24.77
SoUd
Phase.
a
96.4
b+2b^
b
a
u
tt
II
a-\-abM
ibui
II
6+36.4
b
V.
Gms. per 100 ui
ns. Sat. Sol.
Solid
Ba(NOi)i.
KNO».
Phase.
25*
6.62
14.89
a+a6^
25
5-49
16.30
ab^
25
3.04
21.99
u
25
2.04
27.76
b-^ab^
35
"39
0
a
35
8.18
12.99
u
35
8.08
17,48
a
35
8.42
19.75
a+a6.a
35
5-85
24
abut
35
5.02
26.05
««
35
3.02
34.87
b-^abM
35
1.77
34 98
b
35
0
35.01
w
•
Results by FooU.
Ba(NO.),, 2b.a = 2KN0i.Ba(N0i)i, b = KNO,.
Solubility of Mixtures of Barium Nitrate and Sodium Nitrate in Water.
^ , (Coppadoro, at o", 191a; at 30', 19x3)
Results at o^. Results at 30''.
Gms. per 100 Gms. Sat. Sol.
&a(N0i)t.
SoUd Phase.
Ba(N0|)s
II
M
I. NaNOi.
4-33 0.41
3-34 1.68
2.50 3-54
.60 8.02 «
.56 12.71 -
.53 20.24
.56 27.74
.55 30.81
•49 35.83
.55 40.85 9« %Ba(N0,)«+ a %NaN0i
.55 41.30 26 % " +73.8%
.54 42.06 a.6% " +974%
0.51. 41.68 o % " +100 %
Gms. per 100 Gms. Sat. Sol.
Solid Phase.
Ba(N0^
II
u
t<
II
Ba(N0i)s. NaNOi.
10.33 o
8.58 2.33
5.28 7.09
3.89 12.07 "
3.54 14.41
3.20 17.87 "
3.07 19.06 ••
2.81 23.55
2.27 41.22 "
2. II 48.22 Ba(N0i)t+NaN0fe
I 48 . SO NaNOi
o 49 . 16
117 BABIUM NITRATE
SoLUBiLrrY OF Barium Nitrate in Aqueous Solutions op Nitric Acid at 30^.
(Masaon, 191 1.)
Gm3.perxoo0cSat.Sol. - _ Gzns.DerxooocSat. Sol.
^Gr.
'HMOt.
BaCNCW^
Sp. Gr.
HNO..
Ba(N0,)'».
1. 0891
0
54-31
I 0633
73.54
16.66
I.081I
8.303
30-50
1.0668
98.40
15.33
• • •
15-72
27-73
1.0783
125.9
14.99
1.0663
31 -49
22.76
X . 1050
188.6
14. 11
I. 0619
47.18
19.71
I . I34I
251 -6
13 -75
1.0609
63
17.84
I . 164s
315-7
13.52
Fusion-point curves (solubility, see footnote, p. i) are given by Harkins and
Clarke, 191 5i for the following mixtures:
Ba(NO,), + NaNO, + KNO,. Ba(NO,), + NaNOi, Ba(NO,),'+ KNOi,
Ba(NOi)j + LiNO», Ba(NO,)i + UNO, + KN0|.
Solubility OF Barium Nitrate in Aqueous Solutions of Ethyl Alcohol at 25^
(D'Aqs and Siller, 19x3.)
Gms. GiHiOH Qms. per too Gma. Sat. Sol. Cms. CiHiOH Oms. per 100 Gms. Sat. Sol.
pet xoo Gms. <_ -._ ^-- ^ _ .--.— ^ » per xoo Gms. ±1 •' ^,' ^ ^ ^.^ >
advent. OHaOH. Ba(N0|)i. Solvent. C»HiOH. Ba(N0i)i.
o o 9.55 58 57 1.8s
10.25 9.5 7.63 78.7 78.2 0.62
18.6 17.5 6.02 90.1 89.9 0.18
2505 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
oc. and densities are omitted, no exact comparison can be made with the above.
Solubility op Barium Nitrate in Aqueous Phenol Solutions
AT 25^
(Rothmond and Wibmon — Z. phyiak. Chem. 40, 630. 'oa.)
G. Mob, per liter. Gms. per liter. G. Mols.^ per liter. Gma. per liter.
C^H^H Ba(NO«>t. CAOH. Ba(NO»),.' Q»H|OH. Ba(NOi)i. c5So1lb55^»
0.000 0.3835 0.0 100.2 0.310 0.3492 29.12 91.31
0.04S 0.3785 4.23 98.97 0.401 0.3400 37.73 88.90
0.082 0.3746 7.71 97.95 0.501 0.3299 47.11 86.26
0.146 0.3664 13.73 95.81 0.728 (sat.) 0.3098 68.45 3i.oo
Data for the above system are also given by Timmermans (1907).
100 gms. hydroxylamine dissolve 1 1 .4 gms. Ba(N03)s at 1 7**-i8**. (de Bruyn. x89a.)
100 cc. anhydrous hydrazine dissolve 3 gms. Ba(NQi)t at room temp.
(Welsh and Brodetsen, X91S.)
100 gms. methyl alcohol dissolve 0.5 gm. Ba (NOa)* at 25®. (D'Ans andLSiegler. X913.)
100 gms. acetone dissolve 0.005 gm- Ba(N03)t at 25**.
BABIUM NITBITB Ba(N0i)t.H20.
Solubility in Water.
(Oswald, X914; see also, Vogd, X903-)
«•. Gms.Ba(NOi)i -,.. Gnu. Ba(NO0i c„im
— 1.7 9.2 Ice 20 40.3 Ba(NO^t.H^
5 " 43 50.3
I " 6i 58.6
5 " +Ba(NO0i.H«O 80 67.3
9 Ba(N0^)s.Hi0 92 7 1. 7
+ 17 40* ** 1 10 82
* i of the sat. solution « x.4897.
3.2 19
5-8 33
6-5 34
4-3 • 34
u
u
BABIUM NITftlTB
xi8
Solubility of Mixtures of Barium Nitrttb and Silvbr Nitritb in
Water at I3.5^ (Oswaid, 19x4.)
Gms. per loo Gms. HiO.
WnO,).. ' AiNS Solid PhMC.
64 10.2 AgN02+BaAg2(NOj)4.H,0
75-6 9 5 Ba(NOj),+BaAg2(N02)4.H,0
Solubility of Barium Nitrite in Aqueous Alcohol Solutions at
i9.5'*-20.5*'
% alcohol in solvent: 10 20
Gms. Ba(NO,)a.H^ j
per 100 cc. sat sol. J ^^''^ ^''^
BABIUM OXALATE BaC^O^.
Solubility op the Three Hydrates in Water.
(Groflchuff— Ber. 34, 3318, 'ox.)
(Vogel, 1903.)
30 40 SO
60
70
80
90
184 13-3 9-1
4.8
2.7
0.98
0
B&Ca04^H>0.
t«. Gms.BaCs04 G.M.BaCzOi
xooo g. Sol.
0.058
0.082
O.II3
0.170
per 100 Mol.
HsO.
0.00046
0.00066
0.00090
O.OCI36
BaC»0«.aHaO.
Cms. BaCsOA G. M. BaCjO;
per 100 G. M.
HsO.
BaCa04.|HsO.
per
xooo g. SoL
Gros.BaCsOA G.M.BaC|04
per xoo Mol.
0.053 0.00042
per
xooo g. Sol.
0.089
0.089
O.I2I
0.152
0.169
0.00071
0.00097
0.00122
0.00135
0.212 0.00170
9!
18
30
40
45
SO
S5
60
6S
73
75
90
xoo
The following additional data for the solubility of the above three hydrates in
water are given by (Kohlrausch, 1908).
• • •
• • •
o 250
0.285
0.00200
0.00228
« • I*
0.124
0.140
0.151
■ • •
0.164
• • •
O.I7S
• . •
a • •
0.188
0.200
0.2II
H3O.
0.00070
• • •
0.00099
O.0OII2
O.OOI2I
• • •
O.OOI3I
...
0.00140
O.OOI5I
0.00160
o 00169
BaCiOi.3iHsO.
BaCsOi-aHsO.
BaCaOi-iHsO.
f.
2.07
16. 1
17.8
Gms. per Liter.
0.0553
0.059
0.0962
0.1047
f.
3
S-47
11.28
17.9
23 -3
28.4
Gms. per Liter.
0.0519
0.057s
0.0693
0.085
0.0987
O.II24
V.
0.08
2.46
9.62
IS 04
17 54
27.02
33-73
Gms. per Liter.
0.0499
0.053
0.0619
0.0699
0.0751
0.091
O.IO18
Cantoni and Diotalevi (1905) obtained higher results than either of the above.
Solubilities of Barium Oxalate (BaCjOi-iHtO) in Aqueous Acetic Acid at
26**-27**. (Herz and Muhs, 1903.)
Normality G. Rcddtie* Gms. perioocc. Solution. NormaHty G. Residue*
"^ ^^r- CH.C00H. oH.^ "j^ ^^.^
o 0.0077 0.00 0.0154 3.85 0.0564
0.565 0.0423 3.39 0.0845 5.79 0.0511
1.425 00520 8.55 0.1039 17 30 0.0048
a. 85 0.0556 17. II o.iiii
• Dried at 7o^
Gms. per xoo cc. Solntkn
» * >
CHiCOOH. Ba Oxalate
23.12
34 76
103.90
O.II27
O I02X
00096
119 BARIUM OXALATE
BA&IXTM AOID OXALATS BaCaO«.H,C,04.2H,0.
Solubility in Water.
(Gro8chu£F.)
f. ^
rim. per 100
umfl. Mittoon.
Mou. per zoo
Mob. H2O.
Mo]s.HsC,
w
HiC«0«.
BaCsOil
H/:,04.
BaCa04. '
per I Mol3a<
o
0.27
0030
0.054
0.0024
22
i8
0.66
0.070
0.130
0.0056
24
20.5
0.76
0.076
0.15
0.0061
25
38
1. 61
0.16
033
0.013
25
41
1.82
0.18
0-37
0.015
25
S3
2.92
0.31
0.60
0.026
24
60
360
0.40
0.7s
0033
22.5
80
6.21
0.81
1-34
0.070
19
90
7.96
I. II
I -75
0.098
18
99
10.50
I 55
2-39
O.I4I
17
BARIUM OXIDSS.
Data for the lowerine of the fusion points (solubility, see footnote, p. i), of
mixtures of BaO and BsOs are given by Guertler (1904). Results for mixtures of
BaO and CaClt and for BaO and SrCls are given by Sackur (1911-12).
BARIUM Glycerol PHOSPHATES.
Solubility in Water.
Gms. Anhy-
t*. Compound. Formula. drous Salt per Authority.
100 Gms. Sat. Sol.
21 Barium Glycerolphosphate BaCaiiOtP.H<0 4.5 (Rogier and Fiote, igr^.)
13 " a Glycerolphosphate BadHiOtP 1.4 (King and Pyman, 1914.)
12 " fi " BaCsHiOdP.iH^ S.S
2X " Glycerolphosphate BaOHiOtP.iH^ 8.4 (Langbeld and Oppmann, igxs.)
22 " di Glycerolphosphate 3.76 " "
BARIUM PIGRATE. Solubility in HiO + CsHcOH at 25^ (Fischer, 19x4.)
BABIUM PROPIONATE Ba(C,H«0,),.H,0, also 6HA
Solubility in Water.
(Kxasnicki — Mcoatsh. Chem. 8» 597, '87.)
Gms. Ba(C^HsOs)a Gms. BaCCsHiO^s
%\ per loq Gms. f«, per lop Gms.
Water. Soludon. Water. Solution.
o 47-9^ 32-41 SO 62.74 38.57
10 51 56 3402 60 64.76 39.31
20 54.82 35.42 70 66.46 39.93
30 57-77 36.65 80 67.85 40.42
40 60.41 37*^ *• *** ***
100 cc 95% ethyl alcohol dissolve 0.1631 gm. barium propionate at room temp.
_ (CtowcU, 19x8 )
BABIUM SALICYLATE Ba(C«H40HCOO)2.HtO.
100 gms. sat. aqueous solution contain 28.65 S^s. anhydrous salt at 15° and
54.08 gms. at 100®. (Tarugi and Chccchi, X90X.)
BABIUM DinitroSALICTLATE. Solubility in HtO + CtH<OH at 25^
_ _ (Fischer, X9X4.)
BABIUM SnJGATE BaSiOs.
Fusion-point curves (solubility, see footnote, p. i) for mixtures of:
BaSiOi+CaSiOs and BaSiC+MnSiOj are given by (Lebedeu, 191 1).
BaSiOi+LiiSiOi and BaSiOj+NajSiO* are given by Wallace, 1909.
BaSiOi+BaTiC^ are given by Smolensky (1911-12).
BARIUM 8TIARATE
ido
BARIUM STEARATE and Salts of Other Fatty Acids.
Solubility of Barium Stearate, Palmitatb, Myristatb and Lauratb
IN SbVSRAL Solvents. (JacolMon and Holmes, 1916.)
Solvent. t*. Gms. Each Salt (Determiaed Separately) per 100 Cms. Solvent
BaStearate.
Ba PalmiUte. Ba Myristate.
BaLaurate.
Water
IS -3
0.004
0.004
0.007
0.008
ii
SO
0.006
0.007
O.OIO
O.OII
Abs. Ethyl Alcohol
16.5
0.006
0.009
0.009
O.OIO
a ii
SO
0.003
0.004
0.004
0.007
Methyl Alcohol
IS
0.042
0.04S
O.OS7
0.084
(( i(
50.S
0.077
0.088
0.108
0.163
Ether
25
O.OOI
.0.001
0.003
0.007
Amyl Alcohol
35
0.007
0.008
0.009
0.009
BARIUM 8U00IKATB and BARIUM ISO 8U00INATB
Ba.CH,CH,(COO),. Ba.CH,CH,(COO),.
Solubility op Each in Water.
(Miczynskl — Mooatdi. Chem. % 163. x886.)
O
ZO
20
30
40
50
60
70
.80
GmB. Ba. Succinate
per lop Gma.
Water.
0.421
Gms.Ba.
laoSaodnale
per
100 Gms.
Water.
Solatkni
1.884
1.849
2.852
2.774
3 618
3-493
4. 181
4. 014
4542
4 346
4.700
4.656
4-594
4-450
4.410
4.224
3.962
3.810
Accinat
e at 18^ and 0.410
Solution.
0420
0.432 0430
0.418 0.417
0-393 0-392
0.366 0.365
0-337 0.336
0306 0.305
0.273 0.272
0.237 0.237
100 gms. H3O dissolve 0.396 gms. Ba Succinate at 18^
gms. at 25°.
100 gms. 95% alcohol dissolve 0.0015 gms. Ba Succinate at 18® and
0.00 1 6 gms. at 2 5^. (Partheil and HQbner — Arcfaiv. Pharm. 241* 4i3« '03.)
Canton! and Diotalevi (1905), iaind Tanigi and Checchi (1901), obtained data
in close agreement with the above.
BARIUM SULFATE BaSOi.
Solubility in Water. (Kohixausch, 1908.)
One liter of sat. solution contains 0.00115 gm. BaS04 at 0°; 0.0020 gm. at 10^;
0.002A em. at 2&* 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 loo^
Kohlrausch obtained the following results for the solubility of heavy spar
(BaSOi); 0.0019 gm. at o^, 0.0023 K^n* at 10^; 0.0027 P^* at 20^; 0.00315 gm
at 30° and 0.0033 gm. at 33.5**.
100 gms. sat. solution of BaS04 in 21.37% aqueous ammonium acetate solu-
tion contain 0.016 gm. at 25^. (Marden, X916.)
Solubility of Barium Sulfate' in Aqueous Solutions of Iron, Aluminium
AND Magnesium Chlorides at 2o''-25®. (Frapa, 1901.)
Gms.
Chloride
per Liter.
25
Gms.
Chloride
Milligrams BaSOt per liter in:
per Liter. Aq. FeCb. Aq. AlCU. Aq. MgQa.
I 58 33 30
2i 72 43 30 50
5 IIS ^ 33 100
10 123 94 33
Mgs. BaS04 per liter in:
Aq. FeCla. Aq. A1C1«. Aq.Mgda.
150
160
170
• • •
116
170
• •
so
SO
SO
121 BARIUM SULFATE
S0E.TJBILITT OF Barium Sulfate in Aqueous Solutions of Hydrochloric
AND of Nitric Acids.
(Banthisch, 1884.)
In Hydrochloric Add. In Nitric Add.
,-— -^ -\ / * >
cc. containing Mgs. B4SO4 Gms. per 100 cc. cc. cootaining Mgs. BaSO« Gms. per xoo cc
1 Mg. EquiT. per 1 Mg. Equir. Solution. i Mg. Equiv. per i Mg. EquiT. Soltttion.
cTHa. of Ha. Ha. BaSO*: o«HNb». ofHNO*. fiNO». B4S0;.
2. 0133 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 o-S 0.085 12. 6i 0.0170
0.2 0.017 18.23 0.0086 0.2 0.048 31*52 0.0241
100 CC. HBr dissolve 0.04 gm. BaS04; 100 cc. HI dissolve 0.0016 gm. BaS04
at the boiling point. (Haslam, x886.)
Soi^UBiLiTY of Barium Sulfate in Concentrated Aqueous Solutions of
Sulfuric Acid at 20®.
(Von WdnuLrn, 19x1.)
Gms. EbSOi per
Gms-BaSOiper
zoo cc Sat. Sol.
Gms. HiSOiper
Gms. BaSOt jw
zoo cc Sat. Sol.
zoo Gms. Solvent.
xoo Gms. Solvent.
73.83
0.0030
85.78
0.3215
78.04
0.0135
88.08
I.2200
80.54
0.0285
93
«
• • ■
83.10
0.0800
96.17
4. 9^5
84. IS
...t
96.46
18.6900
• Sofid Phase -BaSO«(EaSO0a.HiO + BaSOi.HsSO«. f Solid Phase - BaS0« + BaSOiJB^SOi£«0.
Data for the above system are also given by Volkhouskii (1910).
100 cc. sat. solution of BaS04 in abs. HsS04 contain 28.51 gms. BaSOi, solid
phase s BaS04.3oHsS04. (Bergius, 19x0.)
100 cc. of sat. solution of BaS04 in 95% formic add contain o.oi gm. BaS04
at 18.5^ (Aschan, xgxj.)
Fusion-point curves (solubility, see footnote, p. i) are given the following
mixtures of barium sulfate and other salts:
BaS04 + NaCl (Sackur. X9zz-za.)
" + KCl
" + CaClj
" + KtS04 (Gxahmann, 1913; Cakagni, Z9Z3.)
" + LisS04 (Cakagni and Karotta, Z9zs.)
•f NatS04 (Calcagni. i9za.)
II
BABIUM Amyl SULFATE Ba(C»HiiS04)2.2H«0.
Solubility of Mixed Crystals of the Active and Inactive Salt in
Water at 20.5'*.
(Marckwald, 1904.)
Gms. Saltper Per cent Active Salt Gms. Sak per Per cent Active Salt
100 Gms. HsO. in Dissolved Salt. zoo Gms. HsO. in Dissolved Salt.
28.2 100 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]i>= +2.52**.
BARIUM SULFATE 12a
BABIX7M Isoamyl SULFATE Ba(C»HuSO4)t.2Hs0.
100 gms. H2O dissolve 9.71 gms. of the anhydrous salt at 10^, 11.85 S^s* ^t
19.3^ and 12.15 RTOS- at 20.5^ (Maickwald, 1902.)
BABIUM PerSULFATB BaSi084H^.
100 parts water dissolve 39.1 parts BaSaO, or 52.2 parts BaSaOg.
4H,0 at o^.
(Manhall — J. Ch. Soc. S9$ 77Zt 'OU
BABIUM SULFITE BaSOt.
Solubility in Water and in Aqueous Sugar Solutions.
(RofowioE — Z. Ver Znckerind. 938, 1905.)
Cone, of
Gm. BaS04
per 100 cc. Sol.
CODC. of
Sugar Sol.
Gm. BaSOi
at ao"*.
ESL
100 cc. Sol.
Sugar Sol.
at aof*.
atSo*.
at8o\
o^Bx
0.0197
0.00177
40** Bx
0.0048
0.00158
ID*' "
0.0104
0.0033s
So^ "
0.0030
0.00149
20^ "
0.0097
0.00289
60^ " (sat.)
0.0022
O.OOII2
3o« "
0.0078
0.00223
• • •
...
. • •
r.
perxoooSa. Authority.
HiO.
21. 5
0.27 (B<v]e, 1909.)
20
20
0.522
0.016 (Sandquist, Z91S.)
20
0.03
20
17.5
0.13
3.31 (Meyer, Z875.)
BABIUM SULFONATES.
Solubility of Several Barixtii Sulfonates in Water.
Gms. Anhy-
Salt. Formula.
Barium:
3.4 Diiodobenzene Sulfonate CiiH«oa«SiBa.IbO.
2.5 " " CnEb0iI«StBa.4|H^
2 Phenanthrene Sulfonate (CMHiSOk)tBa.iHflO
3 " " (CMHtS0i)iBa.3Hj0
10 " " (Ci4H,SOi).Ba.3H*0
Bromobenzene Sulfonate (CABrSOOtBa
BABIUM TABTBATE Ba(C,H,0,),.
Solubility in Water.
(Cantoni and Zachodgf — Bull. soc. chim. [3] 33* 75if '05; see also Partheil and Hflboer.)
Gms. Ba(CsHiOfe)s Gms. BaCCtHiOfeh Gms. Ba(CsH^>^
t*. per xoo cc. t*. per 100 cc. t*. per 100 cc.
Solution. Solution. Solution.
o 00205 30 0.0315 70 0.0480
10 0.0242 40 0.0352 80 00527
20 0.0279 50 00389 85 00541
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 i6^
Gms. Ba(CiH«O0i per 100 cc Sat. Sol. in: Gms. Chlo- Gms. Ba(CtH«0«)iper 100 cc. Sat. Sol in:
f.
7%KCL
7% NaQ.
7 % NHiQ. Cvms. Solvent.
KQ.
NaQ.
NHiQ.
16
0.0823
0.0887
0.1050
o.S
0.0398
0.0410
0.0441
30
O.IOI7
O.II5I
0.1370
I
0.0466
0.0514
0.0589
55
0.1230
0.1348
0.1590
3
0.0723
0.0826
0.0892
70
0.1500
O.1781
0.2030
lO
O.II99
0.1260.
0.1342
85
0.1828
0.2168
0.2360
15
0.1435
0.1440
0.1585
20
0.1466
O.IS73
0.1663
(See Note p. asa.)
123 BARIUM TABTR/LTB
SOLUBIUTY OF BASIUM TaRTKATE IN AQUEOUS ACETIC AciD SOLUTIONS AT
26*^-27°.
(Hen and Muhs, 1903.)
Normality Cms. residue* Cms. per xoocc.Solutioii» Normality. Cms. residue* Gms.per loocc. Solution.
of Acetic per 50 cc. ^,t ^^v^tt * t^ ' o» Acetic per 50 cc. *-„ r^r^r^„ * ^ . -J^T"*
Add. Sol. CH«COOH. Ba tartrate. Add. Sol. CH»COOH. Ba tartrate.
0 0.0328 o. 0.0655 3.77 0.1866 22.62 0.3728
0565 O.II51 3.39 0.2300 5.65 0.1865 33.90 0.3726
1 425 0,1559 8.55 0.3115 16.85 0.0218 loi.io 0.0436
2.85 01739 17. II 0.3475
• Dried at 7'^'»
100 grams 95% alcohol dissolve 0.032 gm. Ba tartrate at 18° and 0.0356 gm.
at 25^. (PartheU and Hubner.)
BABIX7M P TBUXILATE. BaCisHi404.2H20.
100 cc. sat. solution in water contain 0.028 gm. of the salt at 26°. (dejong, 1912.)
BEHENIC ACm CsiH4sC00H.
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures of behenic icid and otner compounds.
Behenic Acid + Erusic Acid (Maacarelli and Sanna, 1915.)
H- Isoerusic Acid " "
+ Brassidinic Acid " "
+ Isobehenic Acid (Meyer, Brod and Soyka, 19x3.)
Methylester+Isobehenic Acid Methyl Ester. "
i< <i
BENZALANILINE QHsCH :N.C«Hfi.
Solubility data determined by the freezing-point method are given by Pascal
and Normand (1913), for mixtures of benzafaniline and each of the following
compounds: Azobenzene, benzylaniline, dibenzyl, hydrazobenzene, stilbene and
tolane.
BENZALAZINE C«HfCH:N.N:CHCeHf.
Solubility data determined bjr 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.
BENZALDEH7DS CeHsCHO.
100 gms. HjO dissolve 0.3 pn. CaHj.CHO at room temp. (Fluckinger, 187s; U. S. P.)
Freezing-point data for mixtures of C«H5.CH0 and HNOj are given by Zukow
and Kasatkm (1909).
Para HydroxyBENZALDEHYDS /> CHtOH.CHO.
Freezing-point data are given for mixtures of p hydroxybenzaldehyde -|- di-
methylanuine and p hydroxybenzaldehyde + phenol. (Schmidlin and Lang, 191 a.)
Ortho NitroBENZALDEHTDE 0 C«H4N02.CHO.
Solubility in Water and in Aqueous Solutions at 25®.
(Goldscbmidt and Sunde, 1906.)
Gms. CANOi. Gms. OHiNOi. Gms. OHiNOt
Solvent. CHO per zoo cc. Solvent. CHO per zoo cc Solvent. CHO per zoo
Sat. Sol. Sat. Sol. cc. Sat. Sol.
HjO 0.2316 I nNaCl 0.1899 i nKNOs 0.3199
o.snHCl 0.2391 2 » " 0.1390 2 » " 0.3419
in" 0.2466 o.5»HN08 0.3207 o.5nNaN03 0.3013
2 n " 0.2658 I » " 0.3758 in" 0.3132
1 nKCl 0.2046 0.5 nKNOs 0.3123 2 n " 0.3201
2 n " 0.1912
BSNZALDEHTDE
124
41
<l
U
(I
If
If
41
a
Meta NitroBENZALDEHTDS m C«H4N0t.CH0.
100 cc. HtOdi8Solveo.i625gm.m C«H4N0i.CH0at 25^ (Goldichiiiklt and Simde. 1906.)
I »HC1 " 0.1813
I n KCl " 0.1542
2nKCl " 0.1417
Para NitroBSNZALDEHTDS p aH4N0i.CH0.
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 (Sdmudlin and Lang, x9X9*)
ffi " + Phenol
BKNZALDOXIME C«H»CH:NOH.
Solubility data determined by the freezing-point method are given for mix-
tures of:
a Benzaldoxime + fi Benzaldoxime (Cameron, 1898.)
a Nitrobenzaldoxime + fi Nitrobenzaldoxime. (Beck, 1904.)
BSNZAMIDX
CeH,CONH..
Solubility in Ethyl Alcohol.
(Speyen — Am. J. Sd.U] Z4* 995. '09.)
Sp. Gr. of
IvHons.
5p.C
Soli
O
10
20
25
30
0.833
0.832
0.833
0.83s
0.838
G. M., Gms.
CACONHs CACONHs
per TOO GJhi.. per 100 Gms.
CAOH.
8. IS
CaH^H.
4.2
5-9
6.8
8.2
II
21
04
52
87
56
40
SO
60
70
Sp. Gr. of
Solutions.
0.848
0.862
0.881
0.913
G.M.
C«H«CO
per 100 G.
CflH^H.
II. O
14.2
17.2
20.4
Gxns.
CsHcCONHi
per 100 Gms.
CsEl^H.
28.92
37 •34-
45-22
53-63
Solubility op Bbnzamidb in Mixtures op Alcohol and Watbp
AT 2 5^
CHoUeman and Antiutch — Rec. trav. chim. X3» 394, '94.)
Alcohd.
Gma.
CeH^ONHs
per 100 Gms.
Solvent.
Sp. Gr. of
Solutions.
Vol.%
Alcohol.
Gms.
CsHsCONHs
per 100 Gms.
Solvent.
23 87
18.98
13 -74
8.62
Sp. Gr. of
Solutions.
5-33
2.28
1-35
100 17 03 0830 70
9S 21.12 o.8s6 60
90 34. so 0.878 so
8s 26. IS 0.89s 40
83 26.63 0.900 31
80 26.43 0.907 IS
75 25 41 0.917 o
See radttks imder a AcetoaphtfatHde, |i. xs«
100 gms. pyridine dissolve ^1.23 gms. benzamide at 20^-25^
100 gms. ac^. 50% pyridine dissolve 39.15 grns. benzamide at 20*-25*.
The coefficient of distribution of benzamide between oil and water is 0.66 at
3® and 0.43 at 36**. (Meyer, xgoo, 1909.)
BENZANILIDE.
Solubilities determined by the freezing-point method are given by Vanstone
(19 1 3) for mixtures of benzanilide and each of the following compounds: ben-
zil, benzylideneaniline, and benzoin.
Results for mixtures of 0 chlorobenzanilide and p chlorobenzanilide are given
by King and Orton (1911).
0.92s
0.939
0.949
0.958
0.967
0.982
0.999
CDehn, 1917.)
125 BINZEMB
BKHZXVX C.H..
Solubility in Water at aa^.
(Hen — Ber. 31, 3671, '98.)
100 cc. water dissolve 0.082 cc. C,He, Vol. of Sol. — 100.082,
Sp. Gr. — 0.9979.
100 cc. CeHe dissolve 0.2 11 cc. HjO, Vol. of sol. — 100.135,
Sp. Gr. - 0.8768.
Solubility op Water in Benzene.
(Groachuff, zgzz.)
±m Gm. BaO per zoo «• Cms. HiO per zoo
*^' Gins.Sat.SoL *' Gnu. Sat. Sol.
3 0.030 55 0.184
23 0.061 66 , 0.255
40 0.114 77 0.337
Benzene, Aq. Alcohol Mixtures; Benzene, Aq. Acetone Mix-
tures AT 20®.
H2O added to mixtures of known amotints of the other two and
appearance of clouding noted.
(Bancnrft — Phya. Rer. 3, 31, 1895.96.)
C JI.,C,H.OH and HaO C,H„CH,OHandH,0 C,H„(CH,),COandH,0
Per 5 cc. CtHsOH. Per 5 cc..CH«0H. Pter 5 cc. XCH^)iCO.
cc. HiO. cc. CcH«. cc. HiO. cc. C«H«.
5.0 0-15 8.0 O.IO
3.0 0.215 3.0 0.39s
2.0 0.59 2.0 0.69
1.4 I.O Z.3 I.O
i.o 1.9 0.51 a.o
0.8 3.0 0.295 3.0
0.69 4.0 0.2 4.0
0.49 8.0 0.15 5.0
CtHiOH added to mixtures of known amounts of QHe and HtO until the
solutions became homogeneous at 20**. (LiBcoln, 1900.)
Per s cc. CtH<. Per s cc. CtH». Per 5 cc. C>H«.
ocBbO. ccCtHiOH. ccHsO. cc. CaHiOH. cc. H^. oc. QHiOH.'
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, ethvl alcohol and glycerol and for mixtures of
benzene, ethyl alcohol and lactic acici are given by Rozsa (191 1).
Mutual Solubility of Benzene and Carbon Tetrachloride.
(Determined by the synthetic method.)
(Baud, 1913.)
A» Cms. CiHi per zoo m Gms. CVHi per zoo a. Gins.CiHiperioo
* ' Gms. Mixture. * * Cms. Mixture. ^ ' Gms. Mixture.
—24.2 o —40 19.3 —20 48
—30 2.8 —34 24.2 —10 64.1
—40 8.5 -35tr.pt. 31 o 85.3
— 46.3Eutec. 12.9 —30 36 + 5.5 100
cc. HiO.
cc. CfH^.
20
0.03
8
013
4
0-39
2
1. 17
i-S
1.87
1.0
3S7
0.605
8.0
0.34
20.0
14
126
Mutual Solubility of Benzene and Chloroform. Freezing-point
Method. (Wroaynski and Guye, 19x0.)
Cms. CtHi CrtiM Gms. CeH* q^ijj Gms. CiHi c,ma
f. pcrxooGms. p^ f. per 100 Gms. pifj^ **• Pw i«> Gms. p^*^
Solution. ^*»***^- ^lution. *^***«^- Solution. ^^'^'
— 63.5 O CHCU —60 26.8 aa —20 58.3 CsBt
—70 II. 8 " —50 32 " —10 70.8
-75 14.7 " -40 39 " o 88
— 81.7 18.4 CHCU+OH. —30 47.8 " S 100
— 70 22.6 CiH«
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 COs.
Mutual Solubility of Benzene and Formic Acid. Synthetic Method.
(Ennis, i9X4-)
rof Gms. HCOOH V oi Gms. HCOOHper t^of Gms. HCOOH
Mitdbility per xoo Gms. Sol. Misdbility. xoo Gms. Sol. Miscibility. per xoo 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
SO 16.5 72 60 5 89.6
60 22 70 65
Solubility of Benzene in Aqueous Solutions of Formic Acid. Synthetic
Method. (Ennis. 19x4.)
InosWt. % InSsWt. % In 75 Wt. % In 6o'Wt. %
.HCOOH. HCOOH. HCOOH. HCOOH.
I« ^£ Gms. CiHi |« ^ Gms. OHs ^ ^ Gms. CiHt ^ ^ Gms. CiH«
MisdbUity. ^/Sl. MiscibiUty. ^^^ Wsdmty. cS."^ Misdbility. ^^^
57 S 0-3 71 97 S 122 12 105 6
77 94.4 87 96.6 97.5 8.5 82 3.8
95 89.8 loi 96 74 6 76 3
112 85.2 100.5 14.3
94.5 24.7 81 10
80.5 20 46 7
51 12-5 _
Mutual Solubility of Benzene and Ethyl Alcohol. Freezing-point.
Method. (Viala, 19x4; see also Rozsa, xgxx and Pickering, X893.)
^ Gms. C«H« per ^e Gms. CaHc per m Gms. CcH« per
* ' xoo Gms. Sol. "* * xoo Gms. Sol. ^ ' xoo Gms. SoL
— 113. 9 o —60 19.3 —10 57.6
— 100 8 —50 24.1 o 85
— 90 10 —40 29.8 I 93
— 80 12 -30 37 5.5 100
— 70 15 -20 45.7
Mutual Solubility of Benzene and fi Naphthalene Picrate,
C«H,(NOj),OH.C,oH70H. (Kuriloflf. X897.)
Synthetic method used — see Note, p. 16
^0 Gms. Gms. „ ^.o Gms. Gms. _
* * PicnUe Benzene "" ' Picrate. Bcnxene. ^
157 ICO. ... loo.o III. 6 1-173 1-^37 192
148.4 2.128 0.115 79.3 102.0 1.087 1.780 II. 2
137-4 1-274 0.170 61. I 29.5 0.390 8.430 0.95
134-2 I 384 0.297 49.3 4.6 I 329 21.80 0.48
126.8 I .019 0.343 38.3 5.02 ... 100. o
a — Mols. P Naphthalene Picrate per 100 Mols. of P Napthalene
Picrate plus Benzene.
Determinations for a large number of isothermes are also given.
I2f
Tbb Ststbm Bbnzbnb, Phbnol and Water at 2$\
(Horibo, 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- Solubility of Phenol in Benzene Solu-
tions Containing Phenol and Vice Versa, tions Containing Water and Vice Versa.
'»
Gms. per 100 Gms.
OHiOH+aib+HiO.
Satunttmg
Phue.
%
Gms. per zoo Gms.
CAOH+OHi+BbO.
Phase.
■•
OHiOH.
OH^
9v
OHiOH. GOIc
1.0002
0
0.198
OEU
• • •
29 . 29 0
CAOH
1.0008
I 059
0.204
II
■ • •
71.63 1.62
u
1 .0021
2.602
0.205
II
• • •
74.5 3
CAOH+aHi
I. 00305
3 526
0.199
•1
I
.0256
69.18 16.33
CA
■ • •
5-65
0.17 aa+OHiOH
0
.9891
55-80 36.13
II
• ■ •
5-953
0.132
OHiOH
0
.9629
44.39 50.56
II
1. 0059
6.516
0.075
M
0
.9142
21.15 * 77-22
M
1.0069
7.683
0.025
II
0
.8818
4.78 94.98
U
1.0073
8.19s
0
II
0
.8764
0 99-95
II
Data are also ^ven for the solubility of phenol as solid phase, in CsHs 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, op
Mixtures of*
+
Benzene and Phenol.
("■*'■'"" and Skirrow, i9>7.)
Gnu. OHtper Solid
100 Gnu. Mixture. Phaae.
O CVHiOH
II. 8
38-2
58-4
67 5
78.3
89
100
rofMdting.
39-4
30
20
10
O
S.4£utec.
2.5
o
2-5
51
II
II
II
II
II
"+CJ1«
OHt
Benzene and Pyridine.
(Hatcher and Skinow, 19x7.)
f of Melting. ^^-^C^IJS^
-39-4 o
-45 10
-SO 17
-55 23.3
— 58 Eutec. 26
-50 31
-40 37.7
-30 46
-20 57
-10 71. s
o 90.5
Solid
Phase.
OHiN
II
II
II
GHs
II
41
II
II
II
Additional data on the system Benzene + Phenol are given by Dahms, 189^;
Patemo and Ampola, 1897; Tsakalotos and Guye, 1910, and Rosza, 191 1. Add*-
tional data on the system Benzene + Pyridine are given by Pickering, 1893.
Solubility op Benzene in Sulphur.
t*.
By "Syntheti
Gms. CeHa per xoo Gnu.
ic Method " see Note, p. 16.
(Alexejew, 1886.)
^0 Gms. Csli$
^ Layer.
140 16
ISO 19
160 2S
164 (crit temp.) ^$
per 100 Gms.
100
no
120
130
S Layer. CA Layer:
6 75
8 72.5
10 70
12 66
CA Layer;
61
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 Benxoic Add, p. 155.)
** -{-o Nitrobenzylchloride (Schmidlm and Lang, 19x2.)
" +Bromoform
" 4- Tctramethyldiamino benz- . I „ ,
hydrol J
" -fBenzhydrol
" -f Nitrobenzene (Dahms, 1895.)
" -jrOftn and p Chloronitrobenzene ) (Bogojawlensky, Winogiadow and Bogolubow,
" -f w Bromonitrobenzene J (1906.)
" +o,m and p Dinitrobenzene (Kremann, 1908.)
" + Carbon disulfide (Pickering 1893.)
" 4" Camphene (Kumakoff and Efremoff, 19x2.)
" 'i'tn Cresol (Kxemann and Borjanovici, 19x6.)
" + Cydohexane (Maicardli and Pestalosca, 1907, 1908.)
" -j" Diphenyl (Waahbixm and Read, X9X5.)
" + Diethylafnine (Pickering, 1893.)
" + Diphenylamine (Bmni, 1898; Dahms, 1895.)
" 4- Ethyl ether (Pickering. 1893.)
" + Ethylene bromide (Dahms, 1895.)
" + Ethylene dibromide (Baud and (^ay, 19x1.)
" + Ethylene chloride (Baud and Gay, 19x0.)
** + Ethylene dichloride (Baud and (kiy, x9xx.)
" -f Menthol ^ (Dahms, x89s.)
" 4- Methyl alcohol (Pickering, X893)
_|_ Naphthalene |(Bnini. 1898; Pickering, 1893; Waahbam and
• " + " +i5Naphthol (Bnmi, 1898.)
" + " + Diphenylamine
" . + Phenanthrene
" + " +Carbazol
" + Paraldehyde (Patemo and Ampola, 1891, 1^7-)
" +o,mandp Nitrophenol j^i^^^' ^^~«~**^ "^ Bogoliibow.
" + Propyl alcohol (Pickering. 1893.)
" + Quinine (Van Itenon-Rotgans, X9X3.)
** + Thiophene (Tsakalotos and (kiye, x9xo.)
" + Bromotoluene (Patemo and Ampola. 1897.)
" 4- 1.2.4, 1.2.6 and 1.3.4 I^"*»t«>-lnr««««n ,n««\
toluene ^(Kiwnann, X908.)
4" Urethan (Pushin and Glagoleva and Maaxovich, 19x4.)
" +p Xylene (Patemo and Ampola, 1897.)
Bromobenzene + Chlorobenzene (Paxal, X9X3.)
" T lodobenzene "
" + Fluorobenzene "
P Dibromobenzene + o Dibromobenzene (HoUeman and van der Linden, 191 x.)
+ P Dichlorobenxene i (Bnmi «d Gonri. 1899, KIbtec «>d Wflrfd. X904-
'^ ( os; Kniyt, x9xa.)
+ p Diiodobenzene (Nagomow, 19x1.)
+ p Bromoiodoben- ) „
<«
zene
a
««
■^^bS^zSS™'"" \0>r^^<^^y
+ p Chloronitroben- [(p^^ew*!. .898.)
«« I l« fl
<«
4-m
+ P Bromotoluene (Bondowski and Bocojawleniki, 1904.)
129
BromoBENZEKES
Solvent.
SoLUBiLmr OF p Dibromobbnzenb INT Several Solvents at 25"*.
(Hildebiaiid« EUe&on and Beebe, X9i7-)
Cms. CsHiBn ip)
per 100 Cms.
Solvent.
36.6
Ethyl Ether 71.3
Hexane
Methyl Alcohol
Benzene
Carbon Disulfide
Gnu. CABn {p)
per 100 Gms.
Solvent.
DiBromoBENZEME (/>)
10.3s
83.8
90
CeHfBr,.
Solvent.
Carbon Tetrachloride
25-9
%\
10
20
30
40
SO
60
70
7S
80
Solubility in Ethyl, Propyl, Iso Butyl Alcohols, btc.
(Scfarfider— Z. phynk. Chem. xz, 456, '93)
Determinations by ** Synthetic Method " see Note, p. 16.
Grams CcH«Brs (P) per 100 Grama Sat. Solutioo in:
CiiUOH. CsHiOH. (CH|)CHX:HaOH. (CaHi)^. CSt.
• • • 2T
CgHf. CtHiBr.
14
19
26
38
S7 6
80.5
94.4
27
40
67
8S
9S
20
30
44
6s
77
94.6
30
38
47
S7
67
77
87
34
43
53
62
72
81
90
34
43
62
71
80
88
22
29
36
4S
S4
67
79
84
90
SoLUBiLrrv op Mixtures op p Dibromobenzbkb and p Dichlorobenzbnb
IN Aqueous Solutions op Ethyl Alcohol
Solvent, 50 Vol. % CjHiOH, /=49.I^
(KQster and Dahmer, 2905.)
Gms. per 100 cc Sat. Sol. MoI. % CABn
in Solute.
OHiBn.
0.484
0.505
0.496
0.477
0.470
0.196
O
OHtCh.
O
0.044
0.084
0503
0.721
1.3"
1. 614
100
89.8
80.7
59-3
S4'4
II. 6
o
Solvent, 90.9 Vol. % CjH«OH, / - 25"
(KOster and Wttrfel, 1904-^5-)
Gma. per 100 cc. Sat. Sol. Mol. % CABn
CiHiBn. C.H4CI1. in Solute.
2.909 o 100
2.674 0.696 94
2.220 2.808 70
1 . 769 4 . 249 49
I. 271 6.237 24
0.67s 6.877 9
o 8.271 O
3
7
I
S
9
Additional data for the above system are given by Thiel (1903).
Tribromo BENZENE, CJIsBrs. Solubility, ^s. per 100 gms. at 20-25®:
In HtO, 0.004; in pyridine, 24.3; in Aq. 50% pyndine , 2.01. (Dehn. 19x7.)
SoLUBiLmr Data, Determined by the Freezing-point Method (see foot-
note, p. i), Are Given por the Following Mixtures.
P Bromochlorobenzene + p Dichlorobenzene (Bruni and Gami. 1899.)
" +0 Bromodllorobenzene (HoUeman and Van der Linden, Z9zz.)
P Bromoiodobenzene + p Diiodobenzene (Nagomow. 191 z.)
o Bromonitrobenzene + o Chloronitrobenzene (Krenuum: Kremann and Ehrlkh. Z908.)
•\-P Bromonitrobenzene (Holteman & de Bmyn, Z900: Narbutt, '05.)
+ 0 " (Narbutt. zgos-)
+ P
+ m Chloronitrobenzene (Hasselblatt. r9Z3: Kiister. z89z.)
+ m lodonitrobenzene (Haaaelblatt. Z9Z3.)
4- fn Fluoronitrobenzene "
+ m Chloronitrobenzene (Kremann, Z908.)
P " +^ " (Kremann. 1908; Isaac, Z9Z3; Kremann &Ehrlic]i,Z9o8.)
41
•f
41
44
44
«4
«4
44
ChloroBUIZINBS
130
ChloroBENZENE aHtCl.
Solubility of Chlorobbnzenb in Sulphuk.
" Synthetic Method, ' '
(Akxejew.)
Grama CeE
see
page 16.
per 100 Gruns.
Sulphur
Layer.
13
18.5
27
ChlorBeD-
Koe Layer.
70
63
53
90
100
no
116 crit. temp.
38
^DichloroBENZENE, C6H4CI2. 0 and m ChloronitroBENZENB, C6H4CINOS.
Solubility of Each in Liquid Carbon Dioxide.
(BQchner. 1905-06.)
^'•Dichlorobenzene.
0 Chloronitrobenzene.
m Chloronitrobenzene.
f.
Cms. p CcHiCls
per 100 Cms.
Sat. Solution.
f.
Gms. 0 OHiClNOi per 100
Gms. Sat. Solution.
Gms. M C6H4CINO1
t*. per zoo Gms. Sat.
Solution.
-33
1.2
-32
I
— I 1.8
— 10
4.2
+ s
7.8
+ 16.5 II. 2
+10
II.4
7
16.5-36 quad. pt.
7.5 38.2quad.pt.
20
22.7
8
.58.8
20 53.2
22
34.4
II
65.8
Solubility of 0, m and p Chloronitrobbnzbnes in Aniline. Deter-
mined BY THE Freezing-point Method (see also p. 77}.
(Kremann, 1907.)
r.
—10
4-10
Gms. Each Compound (Determined Separately) per 100 Gms. Sat. Sol.
0 aH«ClNOi.
m aHiClNOi.
4319 (=31 Mol. %) 21.60 f= 14 Mol. %)
31.67 (=»2i.s
51-30^=39
69.15 (=57
«
II
«
49.29 ('=36.5
«
P aHiClNOi.
27.75 (-18.5 Mol.%)
31.67 ( = 21.5
38.50 (-27
(I
II
Solubility Data, Determined by the Freezing-point Method (see
footnote, p. i), Are Given for the Following Mixtures:
Chlorobenzene + lodobenzene
** -|- Cyanbenzene
" -j- Fluorobcnzene
o Dichlorobenzene + p Dichlorobenzene
P \ + P Diiodobcnzene
-\' p Chloroiodobenzene
1.2.4 Trichlorobenzene + 1.2.3 Trichlorobenzene
** + 1-3.5 "
" + *^' " + 1. 2.3 Trichlorobenzene
a Hexachlorobenzene + & Hexachlorobenzene
p Chloroiodobenzene + P Diiodobenzene (Nagomow. zgti.)
0 Chloronitrobenzene + p Chloronitrobenzene (Holleman and de Bmyn. 1900.)
-|- " (Bogajawlewsky. Winogzadow and Bogolubow, 1906.)
+ Formic acid (Bruni and Berti^ 1900.)
m " + m lodonitrobenzene (Hasselblatt. 1913.)
+ m Fluoronitrobenzene "
+ Naphthalene (Kremann and Rodenis, 1906.)
p " -j- Diphenylamine (Tinkler, 1913.)
4- Naphthalene (Kremann and Rodenb. 1906.)
o lodonitrobenzene + p lodonitrobenzene (Holleman. 1913.)
m Benzene disulf one chloride -\rp Benzene disulf one chloride. (Holleman and Pollak« z9za)
(Pascal. Z9Z3.)
(Holleman and Van der Linden, z9zi.)
(Nagomow. Z9zz.)
(Van der Linden. Z9za.)
tt
•I
li
11
««
II
II
II
fi
I3X
NitroBINZINXS
Mutual Solubilitt of Nitrobbnzbnb and Watbr
(Campctti and Del Grono, 1913; Davis, 1916.)
f.
B«0 Layer.
CANO, Uyer.
f.
20
0.19
99.76
180
40
0.3
99.6
200
60
0.4
99.3
220
80
0.8
99
230
100
I
98.7
240
120
1.3
98.2
241
140
1.9
97.2
242
160
2.8
95.8
244
Cms. CJIiNQi per too Cms.
UiO Uy«r.
CHiNO, Ufa.
4-3
93-7
7.2
91
II. 8
87
iS-8
83
23
7a
26
67
32
S8
244.5 cnt. t. 50,1
Data for the solubility of nitrobenzene in hexane, diiaoamyldeouiQ and Ameri-
can petroleum at preuur«t up to 3000 atmospheres, are given by Kohnstamm and
Timmermans (19 13)-
SOLUBILITY OF O, ffl AND p NiTROBBNZBNB IN WaTBR AND QT PVRIDINB.
(Deho, 191 7.)
Gma. Each Conpound Sepaxately per lop Gnu. Solvent.
f *^ N
» Nitxobcnaene. m Nitrobcnaene. p Nitrobenxene.
0.21+ 2.14+ 1.32+
173 two layers formed 85.3
260 394 S3 . 2
Solvent.
f.
Water 20-25
50% Aq. Pyridine 20-25
Pyridine 20-25
SoLVBiLiTY Data, Dbtbrminbd by thb Frbbzing-point Method (see foot-
note, p. i), Are Given for Ml^xTures of Nitrobenzene and Each of the
Following Compounds:
Ethyl Ether (Tiakalotoa and Guye, 1910.) Mercuric Bromide (MaKarell and AKoIi. 2907.)
Hexane (Tunmennans, 1907. 19x1.) Mercuric Chloride ** ' "
Hezane + Resordne (Timmennans. 1907.) Nitrosobenzene (Jaeger and van Kxtgten, x9ia-)
Isopentane (Timmennans, 1910. 19x1.) Phenol (Dahma, 1895.)
Diethyldiacetyltartrate (Scheuer. 19x0.) Ethylene Bromide "
Menthol '* Naphthalene (Kremann, '04; Kumakov.«<al, '15.)
(m) CeH4(NO0,.
Solubility in Benzene, Brom Benzene and in Chloroform.
** Synthetic Method."
(SdirOder.)
Cms &Ht(NO|)t
per xoo
Gms. CeH4(NOi)s per
»•.
C ' ' '
fc.H,
rms. Sol. m:
QHtDr CHCli
%•, xoo Gms. Sol. in:
C.H,
. C,H«Br
CHCI^.
15
I7S
• • •
22. 2
40 52. C
• 380
42.0
20
26.0
18.5
25 0
50 62.5
47 5
52 S
25
33 0
23.7
29.0
60 71 0
' 57 0
65 0
30
40 0
28.7
33 0
• • • • •
• • •
. • «
SOLUBUm OP :
m DnnTKOBBNZBMB IN Sbvbsal Aloobou ADO AOM
«
(Timofeiew. 1894)
Gms. m
aHi(N0|)t
Sohrent.
Gms.«uai(NOlOi
per too Gms.l
Solvent.
r.
per 100 Ume.
f.
Sat. Sol.
Solvent.
Sat. Sol. Solvent.
CH/)H
13 -8
5-38
S.65
CHiCOOH
^SS
15.7 18.6
CtH»OH
13-8
2.83
2.92
<(
23
17.8 21.6
CHtOH
13 -8
2
2
CtHiCOOH
13s
12 13.6
CHjOH
73
43-6
77.3
((
15s
12.9 14 8
HCOOH
^3-5
9
9.9
<(
23
13-45 ISS
HCOOH
iSS
9.6
10.5
CHtCOOH
135
7.3 8.3
CH,CXX)H
13s
IS-2
17.9
«
^S-5
8.2 8.9
1 00 gms. 95 % formic acid dissolve 1 1 .89 gms. m dinitrobenzene at 20.8^. (Ascban.'xi) .
100 gms. pyridine dissolve 106.3 sms. m dinitrobenzene at 20°-25^ (Dehn, x9x7.)
100 gms. 50% aq. pyridine dissolve 45.5 gms. m dinitrobenzene at 20°-25^ "
NitroBENZENES 132
SolubiHties of Di-Nitro BXVZXVX8 and of Tri-Nitro BXVZXVX8 in
Several Solvents.
(de Bruyn — Rec. txvr. chim. Z3» 1161 150, '94.)
Gnuna per xoo Gnuns Solvenc.
(NO,),. (NO,),. (NO,),. (NO,),. C«)C.Ht(NO^
Methvl Alcohol ao.5 3.30 6.75 0.69 4.9 (16®) 16. a (15.5®)
Ethyl Alcohol ao.5 1.9 3.5 0.4 1.9(16®) 5-45 (15.5 v
Propyl Alcohol ao.5 1.09 a. 4 0.298 ...
(Maroon Bi-Sulphide 17.6 0.236 1.35 0.148 0.25
Chloroform 17.6 27.1 32.4 1.82 6.1
Benzene 18.2 5.66 39<45 2.56 6.2 (16®)
Ether '7*5 *** *** *** '*5 **•
Ethyl Acetate za.2 12.96 36.27 3.56
Toluene 16.2 3.62 30.66 2.36
CarbonTetraChloride i6.a 0.143 '-'^ c>.i2 ...
Water (ord.) 0.014 0.0525 0.008 •••
S3rmmetrical Tri-Nitro BUTZSNE.
Solubility in Aqueous Alcohol at 25®.
(HoUeman and Antusch — Rec. tniT. chim. Z3» 396, '94O
Vol.% ^-^S^^*^'^ Sp.Gr.of Vd.% ^SSr^^?^'^ Sp. Gr. of
AlcolS. ^%i^t Solutions. Alcohol. "^^^f/ Sciurioiif.
100 2.34 0.7957 80 0.57 0.8582
95 1-57 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 0 C«H4(N0s)s, 3.1 gms.
m C6H4(NOs)s and 0.33 gm. p CcH4(N0s)s at 25°. (HoUeman and de Brayn, 1900.)
100 gms. of each^of the following solvents dissolve the indicated gms. of 1.2.4
trinitrobenzene at 15.5°: CeHe, 140.8 gms.; CHClt» 12.87 gms.; CHtOH, 12.08
gms.; (CsHOiOy 7.13 gms.; CsHeOH, 5.42 gms; CSt, 0.4 gm. (de Bmyn. 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 0, m and p dinitrobenzene with fluorene, Kremann (19 11); with phen-
anthrene, Kremann, ei al (1908). Results for mixtures of 0 and p dinitrobenzene
with naphthalene, by Kremann and Rodinis (1906). Data for m dinitrobenzene
with nitrotoluenes are given by Giua (19 15) and for m dinitrobenzene and di phenyl-
amine by Giua (1915a). Similar data for mixtures of x trinitrobenzene with
xanthone, quinol, dimethylpyrone, s 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 (19 10) and for 5
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 (CeH«)tCHOH.
Solubility data, determined by the freezing-point method (see footnote, p. 1)9
are given for mixtures of benzhydrol and phenol and for benzhydrol and di*
methylaniline by Schmidiin and Lang (1912).
(I
I<
«4
133 BENZIL
CeHiCO.COCeH^
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, 19x5.)
" -|- Azobenzene
" +Stilbene
" -|- Hydrobenzoin
" 4- Benzoin (Beunth, 1919-23; Vanatooe, 1909.)
" -h Benzoic acid (Kendall and Gibbons, 1915.)
fiSHZIVX (Petroleum) CsH,,C,Hu.
100 parts of alcohol dissolve about z6 parts benzine of 0.638—*
0.660 Sp. Gr., at 25®.
BXVZOIO AOID C,H,COOH.
Solubility in Water.
(Boorgoui — Ann. chim. phys. [5] zs» i7it '78-)
Gzams. CeHsCOGH Grams. CACOOH
^•, per 100 Gms. t*. per i<x> Gms.
Water. Solutka.
o 0.170 0.170 40 0.55s 0551
10 0.3I0 0.209 50 0.775 0.768
Water.
Solution.
0.170
0.170
0.3I0
0.209
0.290
0.289
0.34s
0.343
0.410
0408
20 0.290 0.289 60 I -155 1*143
25 0.34s 0.343 80 a. 715 2.643
30 0.410 0408 100 5.875 5.549
100 grams saturated aqueous solution contain 0.25 gm. CcHfCOOH at 15^;
0.3^^6 gram at 25**; 0.353 gram at 26.4**; 0.667 gram at 45**; 5.875 gms. at
100".
(Paul, 1894; Noyes and Cbapin, 1808; Greenish and Smith, 190^; HoCFman and Langbeck, 1905: Lums-
den, 1905; Phiup, 1905; see auo Aiexejew, x886; Ost, 1878; Vaubel, 2895; Freunduch and ScaI, i9za.)
Solubility op Mixtures of Liquid Benzoic Acid and Water.
(Alexejew.)
Determinations by "Synthetic Method," see .Note, p. 16. Figures read from
curve.
Gms. CsHbCOOH per zoo Gms. Gms. CeQsCOOH per 100 Gms.
t*. . * s t». . * ^
Aq. Layer. Benzoic Ac. Layer. Aq. Layer. Benzoic Ac. Layer.
70 6 83 100 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:
(Hoflfman and Langbeck.)
Potassium Chloride at 25°. Potassitmi Nitrate at 25®.
^ ia: Dissolved C,HbCOOH. ^ ^; Dissohed C^HaCOOH.
Kol' iS. M0I.C011C. Wt. per cent. ^^ £J^ Mol.Ccnc. Wt.percent
0.02 1.49 5.0254-IO-* , 0.339 002 2.02 5.0326-IO-* 0.340
005 3-73 49801 " 0-333 005 S-06 50421 " 0.341
0.20 14.92 4-7639 " 0.322 0.20 20.24 5.0297 " 0.340
0-50 3730 4.3632 " 0.295 0-50 50-59 4-9400 " 0.334
x.oo 101.19 4.7646 " 0.322
BENZOIC ACm
134
Solubility op Benzoic Acid in Aqueous Solutions op:
(Hoffmann and Langbeck.)
Sodium Chloride.
Sodium Nitrate.
Nor.
Gmg.
Gms. CsHaCOOH
malitf
NaQ
per 100 Gms. Sol.
of Ag.
NaQ.
lite^.
at 25". at 45*-
0.00
0.00
0340 0667
o.oa
1. 17
0.339 0.663
0.05
2-93
0-33S 0.6S4
0.20
11.70
0.336 0.617
0.50
29.25
0 . 282 0 . 546
1. 00
58.30
... 0 . 449
Nor-
mality
GmB.
NaNO,
Gm5.CeH^COOH
per 100 Gms. Sol.
of Aa.
NaN&t.
per
Liter.
at 2f» at 45**.
002
1.70
0340 0.666
005
8.51
0.339 0.66s
0.20
17. 02
0-333 0647
0.50
42.54
0319 0.613
x.oo
85.09
0 . 294
Solubility op Benzoic Acid in Aqueous Solutions op Sodium
Acetate, Formate, Butyratb, and Salicylate.
(Noyes and Chapin — Z. phyaik. Chem. 37. 443t '98; Philip — J. Ch. Soc. 87. 9pa. '05.)
Grams
Sodium
Salt per
liter.
O
I
2
3
4
6
8
Grams CeH«COOH per liter of Solutioa in:
— ^
CIIsCGGNa.
HCOONa.
At 25^
3 41
4 65
S-70
6.70
7.60
At 26.4*.
3 53
4. 75
5-85
6.90
7-85
Atl?7
3 41
425
4-7S
5.20
5 60
At 264*.
3 53
4-35
4.85
S-30
S-70
COIrCOONa. CAOH.COONa.
At 264*.
3
4
5
6
At 264*.
3 53
3.62
3 70
3 -So
387
400
4.10
Solubility of Benzoic Acid in Aqueous Solutions of Sodium Mono-
chloracetatb. Sodium Succinate and Potassium Formate at 25*".
(Philip and Gamer, 1909.)
In Aq. (CH,COONa)j.
Gms. per Liter Solution.
53
50
40
15
6.90
8.40
In Aq. CHiClCOONa.
Gms. per Liter Solution.
CHiClCOONa^
O
1-375
3.426
6.839
13.710
C«H*COOH.
3.38
3.684
4.026
4.417
4.929
(CHiCOONa)i.
O
1. 182
2.932
5.848
11.730
C«H»COOH.
3.38
4.087
5-112
6.564
9OO5
In Aq. HCOOK.
Gms. per Liter Solution.
HCOOK.
O
1.025
2.563
5 124
CtHtCOOH.
3.38
4.087
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.
1 00 cc. 90% ethyl alcohol dissolve 36. 1 gms. C«HiCOOHat i5.5*'.(Greenish&Smlth,*o3.)
100 cc. of a i.o n aqueous solution of aniline hydrochloride dissolve 0.537 fi^<
C«H6COOH at 25°. (Sidgwick, 1910.)
Solubility of Benzoic Acid in Aqueous Solutions of Ethyl Alcohol
AT 25**.
(Seidell, 1908, 19x0.)
CiH«0&
Sp. Gr. of
Sat. Sol.
Gms. per 100 Gms Sat.
Sol.
CiH»6b
in Solvent.
Sp. Gr. of
Sat. Sol.
Gms. per
xoo Gms. Sat.
Sol.
m Solvent.
CiHsOH. CiH»COOH:
CtH^OH.
CrfliCOOH:
0
I
0 0.367
60
0.943
45 72
23.80
10
0.985
9.94 0.60
r •
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 9.10
100
0.908
63.1
36.9
SO
0.946
41.50 17
135
BKNZOIG ACID
Solubility op Benzoic Aao in 90% Alcohol, in Ethbr and in Chloroform.
.(Bouigoin.)
Solvent. t^
' Solvent.
SdudoQ.
p
90% Akohol 15
41.
.62
29 -39
Ether 15
31 '
35
23.86
Chloroform 25
14 30
12.50
SCMLUBILITY OF BENZOIC AciD IN
Several Alcohols.
(Thnofdew
• 1894.)
Akr>ho1.
^ Gins.C«HiCOOHperzooGins.
Alcohol.
.. Gms-CeH^COOHperxooGins.
Sat. SoL Solvent.
Sat. SoL
Solvent.
Methyl
— 18 23.1 30
Propyl
-18
14. S
16.9
«
— 13 24.3 32.1
it
-13
iS-7
18. s
«
+ 3 335 504
<i
+ 3
23.1
30
«
19.2 40.1 67.1
i<
19.2
28.2
39.3
It
23 41.7 71. 5
(f
23
29.8
42.3
Ethyl
— 18 20.3 25.4
Isoprupyl
21.2
32.7
48. s
«
— 13 21.2 26.9
AUyl
21.2
25.1
33-4
«
+ 3 28.8 40.4
Isobutyl
0
15. 3
18
(1
19. a 34.4 52.4
Isoamyl
Capryllic
18
20.2
25-4
M
23 35-9 SS-9
21.2
22.7
28.7
Ethyleneglyool
i 18
8
8.69
Additioni«1 dat». agreeing closely with the above, $re given by Timofeiew
(1891) and Bourgoin (1878), ; . .
Solubility of Benzoic Acid in Aqueous Solutions of Dextrose.
(Hoffman and Langbeck.)
Dissolved CeHsCOGH at sj".
Ncnnality of
m]. Dextruw.
0.02
0.05
0.204
0.533
1. 068
Gma. CaHiiOs
per Uter.
3 67
9.00
36.73
96.15
192 .30
Mol. Cone.
5.0322.10
5 0403 "
((
u
-4
SO303
5 0321
50443
Weiffht
Per Cent.
0.34
034
034
0.34
0.341
Md. Cone.
9.9088.10"*
9.9328
9-9323
lO.OIOI
10.0369 "
Dfasolved QiHgCOOH at 4i*.
Wdfffat
•ter Ctnt.
0674
0.669
0669
0674
0.676
((
«
((
SOLUBIUTY OF BENZOIC AaD IN AOUEOUS SOLUTIONS OF UREA AND OF ThIO UrBA.
(Homnan and Langbeck.)
Ncnnality Gms. CaHaCOOH Dissolved at af,
of Solution. per Liter. Mol. Cone. Wt. percent
In Aqueous Urea o . 10 6 .01 CO(NH2)2 5 . 1876 . lo"* o .350
In Aqueous Thio Urea 0.20 15.23 CS(NI^)3 5*4994 " 0372
Data for the S3^ein benzoic acid, succinic acid nitrile and water are given by
Schreinemakers, 1898, and for the system benzoic add, phenol and water by
Timmemianns, 1907.
SoLUBiLmr OF Benzoic Acid in Benzene and Vice Versa. (Roioff, 1895)
f.
S-37
Cms. CrfbCOOH per
100 Gms. Sat S<M.
0
Solid Phue.
CJEI,
•f-^rSS'.^S^iT' Solid Phase.
20 8.8 GeHBCOOH
5
I-7S
«
30 13
4SO
4.30
S
3-95
5
S-os
• 1
CJli+CHjCOOH
QHsCOOH
SO 25
70 43. S
90 64
7
5 SO
((
no 91.5
9
II
S-70
6
It
It
121 100
Von Euler and Lowenhamn (1916) found 7.76 gms. CeHsCOOH per 100 cc. of sat.
.solution in benzene at 25**, and 7.76 gms. CeHsCOOH + 2.50 gms. C«H40HCOOH
o per 100 cc. of benzene solution saturated with both acids.
BENZOIC ACm
Solubility of Benzoic Acid in Organic Solvssts.
Aq. 75% Acetic Add
14-16
B^QC
14-16
Carbon Disuiede
14-16
Carbon Tetrachloride 14-16
'S
i6
Chlorobrm
»S
Ethyl Ether
14-16
Glycerd
1S-16
Ligroin
14-16
Petrtrieum Ether t
a6
Pentachlor Ethane
*S
Tetrachlor Ethane
15
Tetrachlor Ethylene
as
Trichlor Ethjdeoe
as
Dichlor Ethylene
• . GiM. OHiCOOH per
Bd EIaUeiiiu(i9ii): {1) H
ki(i9o7); (s) WcXciudBmliutiau); (6) Sadell
One liter sat. aol. of benzoic acid in ethyl
37.7 pns. at 21.5** and 95.7 gma. at 75°.
SOLUBIUTY 0
Solution.
Sit. Sol.
Amy! Alcohol
as
0.87s
33.37 {6)
Amyl Acetate
as
0.9 11
M (6)
AloAol (Aba.)
*S
0.^
s8-*o {6)
Benzene
*s
0-8Q7
13.23 (6)
Chloroform
I.4S6
IS-14 (6)
Carbon TetracUoride»s
t.s64
4-18 (6)
Carbon Disulfide
^s
i.iSi
4.82 (6)
Cumene
as
8-59 (6)
Ethyl Ether (Abs.)
as
46.74 6
Ligroin
as
0.710
»-7S (6)
Naphtha
aj
0.730
3.6s (6)
Nitrobenzoie
as
i.aas
M-os (6)
Toluene
as
0.8S4
io.6g (6)
Spts. Turpentine
as
0.8S9
Water
as
Xylene
'5
0.877
g.71 (6)
gm.. HI. «I. t CB
pt-JO-TO.)
ii^R.Uim«iii (I91J): (i) d. J
ng(.9o9)
t4)0»».
Mixtures of Ether
Mixtures of Acetone
Mixtures c
( Ethyl A«-
+ Chloroform.
+ Beniene.
tate + Benzene.
'^ssa'-'^SS^ IS'
Gnu. CJltCOOH
per 100 Gnu.
la!"
Cni.aHJC0OH
100 38.4
100
II.6
100
II.6
90 34
90
18.3
90
14
80 30.1
80
34.1
80
16. s
70 a6
6
70
31
70
20
60 33
9
60
33 S
60
J0.4
50 20
8
50
37
so
32
40 18
6
40
43.3
40
23.9
30 16
8
30
47
30
26.S
30 15
6
SO
49
so
29
10 IS
3
10
Si-3
Id
28.2
0 IS
0
SS.6
41.2
•Tl>i.>.proUI>ly.
akukt Id the orisiiu) and •hnOd be %(aH>)iO in Solvent.
5oi.i;BtLiTY Data, Dbteruinsd bt the
Fhkkzing-point Method (see footnote.
p. i), ARB Givbn fos
MiXTUKBS OF
Benzoic Acm
ANOEiCB
or TBB Fm.-
lowing Compou
NDS:
t CUoTobenaMcAdd
(Bommter tod H
m Nitrobenzoie Add (Bikuoia aiid AngriMsi, I
Benzil (KendiU wd Gibboo*, 19
Camphor (louniiuu, 1911.)
Cinnamic Add (KuUer, iSto; Kndall. 1
DimethylpyroDC (Keadill, 1914.)
Fluorobenzoic Add (Koopd, igiij
Salicylic Add y»er*. ■»«■)
ij.) Sucanic Add Nitnle {Schnk
Sulfuric Add (
o Toluic Acid (KhkUU, igu.)
J a Toluidine (Bukov, igij.)
P- " (Bukov, igii; Vitnoa, iSgiJ
137 BENZOIC AGID
Distribution op Benzoic Acm B&twebn Watbr and Bbnzbnb:
At lo**. At 20**. At 25*. At 40^
(HendrixoD, 1897.) (Nernst, 1891.) (Fanner, 1903.) (Hendrizon, 1897.)
Cms. CACOOH Gma. CtHtCOOH q-^ rjtroOH ner too oc ^ms. CsHiCOOH per
per 100 cc. per xoo cc. \-•Il•^-w« pu iw ^^ ^^ ^^
HsO. OH* HiO. OHt. HsOLayer. CJIc HiO OHc
Layer. . Layer. Layer. Layer. * Layer. Layer. Layer.
0.0215 0.0725 0.0163 0-0535 0.2002 (0.1885*) 3-335 0.0238 0.0714
0.0412 0.2363 0.0244 0.099 0.2012 ro.1891*) 3.349 0.0404 0.1637
0.0563 0.4422 0.0452 0.273 0.2020 (0.1902*) 3.319 0.0837 0.5740
0.0890 1.0889 0.0788 0.737 0.1155 1.0269
0.1215 2.0272 0.1500 2.42 0.1715 2.1420
0.1409 2.7426 0.2890 9.70 0.2313 3.9167
• M unionized.
Distribution of Benzoic Acid Between Benzene and Aqueous
Potassium Benzoate Solutions at 25®.
(Fanner, 1903.)
/. S%Jfe^' Gm- Mob. OHiCOOH per Liter. G«». OaCOOK Cms. GHiCOOH per Kter.
CtHs(X)OKper , , per Liter Aq.
Liter Aq. Sol. Aq. Layer. CsH« Layer. S(d. Aq. Layer. CiH« Layer.
0.0093 0.01587 0.2776 I. 341 1.937 33.88
0.028 O.OIS97 0.2768 4.03s 1.950 33.79
0.047 0.01603 0.2762 6.774 1.956 33-71
Distribution of Benzoic Acm Between:
Water and Chloroform. (Hendiizon, 1897) Water and CCI4. (Seidell, z9zoa.>
At I0^ At 40*. At 25*.
Cms. C<H*C0pH per 100 cc. Cms. CtHiCOOH per loo cc. Gms. CtHtCOOH per 100 cc
H^ Layer. OH* Layer^ HsO Uyer. OH* Layer.' HaO Layer. CCU Layer.'
0.0208 0.0915 0.0258 0.0880 0.134 0.830
0.0269 O.1518 0.0432 0.2059 0.291 4.41
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 (191 1) as 12.6.
AminoBENZOIG ACID (0) aH4.NHs.COOH.
Solubility of 0 Aminobenzoic Acid in Water. (Lunden, 1905-06.)
♦. Sp. Gr. Gms. C6N4NHsCOOH(0) *« Sp. Gr. rinjSSwkTT/>.%
*•• Sat-SoL per 100 cc Sat. Sol. *' Sat. Sol. ^S?^^^
25 0.999 0.519 34.9 0.998 0.731
26.1 ... 0.540 35 0.997 0.744
28.1 ... 0.570 39.8 0.997 0.889
Solubility of Aminobenzoic Acid in Aqueous Salt Solutions at 25**.
(Lunden, 1905-06.)
'"'^SoS!'^* ^^-' ""^^^^^^'^ NonnaUtyof Sp^Gr. cA.
SolutKm. Solution. c^^StS; Solution. Solution. per 100 cc.
bat. boluuon. g^ g^j
0.768 JBa(NQs)2 1.080 0.634 2.633 KNQs iiSS 0.501
0.507 " 1.052 0.603 1.372 " 1.083 0.544
0.3427 " 1.037 0.585 0.598 " 1.033 0.549
0.1780 " 1. 018 0.555 1.853 KI 1. 221 0.541
0.154s " 1.015 0.549 0.946 " I. 114 0.559
0.560 " 1.068 0.556
The author also nves additional data for aqueous salt solutions at 28.1**.
Additional data for the solubility of aniinobenzoic acid in aqueous salt solu-
tions are given by Euler (19 16).
AminoBINZOIG ACIDS
138
AminoBENZOIC ACID aH«.NHi.COOH (m).
Solubility in Water and in other Solvents.
In Water.
■
In Organic Solvents.
Cms.
'
Gms.
t*. CaH«Jm9.COOH(M)
Solvent.
t*. CA-NHs.COOH(m)
per 100 cc. HsO.
per zoo cc. Solvent.
0
043
Ethyl Alcohol (95^)
12.5 3.92
10
0.52
Methyl Alcohol (pure)
10. s 405
20
067
Acetone
II. 3 6.22
30
0.87
Methyl Iodide
10 .0 0.04
40
IIS
Ethyl Iodide
0.0 0.02
SO
I so
Chloroform
12.0 0.07
60
2. IS
Bromoform
8.0 trace
70
31S
•
Mutual Solubility op a
\minobenzoic Acids and Water at High Tempera-
tures, Determined by the Synthetic Method.
(Flaschner and Ranlcin, 19x0.)
Mixtures of 0 AaD
Mixtures of m Acid
Mixtures of p acid and
HjO.
and HfO.
and HsO.
fof
Gms. 0 Acid per
t" of Gms. m Acid per
t* of Gms. p Add per
Melting.
zoo Gms. Mixture.
Melting. xoo Gms. Mixture.
Melting, zoo Gms. Mixture
83.6
4.8
66 crit. sol. temp.
47 crit. sol. temp.
9S.8
9.9
77.8 4.6
82.2 s
101.4
18. 5
90 S.8
90 7.1
103.4
30.6
100 9.7
100 15.8
104.4
38
no 20.2
105 22
los
49-4
120 51.2
no 32.3
105.6
59 -4
130 73-7
1x6 51.8
107.8
69.7
140 83.7
120 62
112
80
ISO 90.7
130 77
116. 2
87.2
160 95.8
150 91. I
128.4
95
170 99.2
170 98
144.6
ICX>
174.4 100
186 100
f 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).
AminonitroBKNZOIC ACIDS CeH,.NOs.NHs.COOH 0, m and p.
Solubility op the Three Isomeric Aminonitrobenzoic Acids:
In Ether.
r.
2.7
S.8
Gms. CeI&.N0,.NHt.C00H per
100 cc. Ether.
Para.
Oftho. Meta.
10.84 1.70 6.41
16.05 (6.8**) i.8i 8.21
f.
3
9.6
In Ethyl Alcohol (90%).
Gms. aHtNO|.NHs.COOH per
100 cc. Alcohol.
Ortho.
8.13
10.70
Meta.
1.79
2.20
Paia.
8.4
"•3
Solubility in Water op the Three Isomeric:
(Vaubd, Z895)
Aminobenzo Sulphonic Acids. Amino Phenols.
r.
7
G. CJI4.NHt.SO1H per zoo G. Aq. Sol.
Ortho. Meta. Para.
1.06 1.276 0.592 (6**)
r.
O
G. aH«(OH).NHs per zoo G. Aq.SoL
Ortho.
1.7
MeU.
3.6(20**)
Para.
I.I
139
BENZOIC ACIDS
Grams.
Gram Mol.
1.856
0.00924
0.402
0.00200
0.056
0.00028
2.087
0.01333
0.952
0.00384
O.I16
0.00047
0.027
(Koopal, 19x3.)
Brom, Chlor and lodoBENZOIC ACIDS.
SOLUBOLITT IN WaTER AT 25®. (Paul, 1894; Ldwenherz. 1898; Vaubel, x89s3
_ , Per xooo cc. Aqueous Solution.
Formula, *
CfftBr.COOH (ortho)
C«H4Br.C00H (meta)
CfftBr.COOH (para)
C6H4CLCOOH (ortho)
CJEW-COOH (ortho)
CJEW-COOH (meta)
CeHJ-COOH (para)
The following results at 28^. (Skger, 19x2.)
Chlorobenzoic add CjHiClCOOH (ortho) 2 . 25
(meta) 0.45
(para) 0.093
Mutual SoLUBiLnY of Bromo and Chlorobenzoic Acids and Water at High
Temperatures, Detebmined by Synthetic METHOD.J^CFiasdmer and Rankin, 19x0.)
p Bromobenzoic o Chlorobenzoic m Chlorobenzoic p Chlorobenzoic
Add + Water. Add + Water. Add + Water. J Acid + Water.
Gms. Acid
per xooGms.
Mixture.
10
Compound.
Brombenzoic Add
Brombenzoic Acid
Brombenzoic Acid
Chlorbenzoic Add
lodobenzoic Acid
lodobenzoic Add
lodobenzoic Acid
it
((
((
t* of Gms. Acid M £
Mdting. I«^JS^«- Melting.
170 (Grit. sol. temp.) I00.8
40 ^ Gms. Add m .£ Gms. Add
Melting. »*L^~ S^- Melting. ^J2lS^
169
180
190
196
200
210
22Q
240
2S4
3
6.2
27
61
80
88.3
96.9
100
102.7
104 20
I26.2(crit.t.)34.9
104 76
no 85.3
120 92
130 96 . 5
139 . 5 100
Mixture.
123 4.2
123.8 18.9
I42.8(crit.t.)34.3
Mixture.
167 (crit. L)
123.8
125
130
140
ISO
75-8
81.5
87. S
93-2
97-S
100
162
170
180
183
184
187
200
220
240
. 3
5.4
10
14.5
"5
47
79. S
92
100
SoLUBiLTTY OF Orthochlorobenzoic Acm IN Aq. Solutions of Sodium Ace-
tate, Sodium Formate and Potassium Formate at 25**. (Philip and Gamer, 1909.)
In Aq. CHiCOONa.
Grams per Liter.
CHsCOONa.
In Aq. HCOONa.
Grams per Liter.
1.009
2.484
5.027
10.07
CtHiGCOOH.
3 599
6. 181
15.60
18.27
HCOONa.
0.843
2.102
4.196
8.410
OHtOCOOH.
3.381
S.258
7-637
11.02
In Aq. HCOOK.
Grams per Liter.
fiCOOK.
O
1.025
2.563
5-124
aH«acooa.
2.128
3 396
5.226 .
7-S43
SoLUBiLmr OP Chlorobenzoic Acms in Several Solvents at 14-16^
(Bomwater and HoUeman, 19x2.)
Solvent.
ligroin
Carbon Tetrachloride
Benzene
Carbon Disulfide
75% Aq. Acetic Add
Ethyl Ether
Acetone
Ethyl Acetate
Gms. per xoo cc. Sat. Solution.
0 OHiaCOOH.
0.07
0.58
0.92
0.52
6.22
16.96
28.42
m OHiaCOOH.
0.084
0.48
0.66
0.62
• • •
14
p CtHiaCOOH.
trace
0.04
0.017
0.016
0.32
1.72
2.58
1.64
13 . 20
Freezing-point data are given by Bomwater and HoUeman (19 12) for mix-
tures of 0, m and p chloroboizoic adds.
BENZOIC ACIDS 140
FluoroBENZOIC ACIDS QH4FCOOH.
100 cc. aqueous solution saturated at 32^ contain 0.882 gm. 0 CeH4F.C00H.
« « 14 4< 14 II Q jQ^ 44 p 14
(Sbtboawer, 1914.)
lodoBENZOIC ACm p QH4ICOOH.
Mutual Solubility of Para Iodobenzoic Acm and Water at High Tem-
peratures Determined by the Synthetic Method,
t* of Cms. Add per
Vol
Cms. Add per
fof
Gms. Add per
Melting. loo Cms. Mixture.
Melting.
100 Gms. Mixture.
Melting.
100 Gms. Mixture
17s crit. sol. t.
207
22
230
87.4
178 3
210
41
240
92.7
190 S-8
2IS
63 S
269
98.1
200 10
220
77
270
100
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.
" +/> Iodobenzoic
p Iodobenzoic " " + P Bromobenzoic " "
HexahydroBENZOIC ACID CH,(CHs.CH,),.CH.COOH.
100 gms. HsO dissolve 0.201 gm. of the acid at 15^, d, saturated solution » 1.048.
(Lumsden, 1905.)
HydroxyBENZOIC ACIDS m and p (0 » 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. C«H«.OH.COOH Gms. C|II«.OH.COOH
♦•. per 100 Gms. HsO. per loo Gms.C6H>.
MeU.
Para.
Meta.
Paia.^
10
OSS
0.25
• • •
0.0018
20
0.90
0.50
0.008
0.0027
as
1.08
0.65
o.oio
0.003s
30
1-34
0.81
0.012
0.0045
35
1.64
1. 01
0.015
0.0060
40
2.10
1.24
0.017
0.0082
SO
3-IO
2. 12
0.028
0.0162
60
• • •
...
0.047
0.028
80
• • •
In Acetone.
• • .
...
In Ether.
0.066
G. C|H«.0HXXX>H
G. C|H«.0H.C00H
%\
per 100 cc.
Sol.
t*. per xoo^cc. Sol.
MeU. Fanu Heta. Para.
23 26.0 22.7 17 9.73 9.43
100 gms. sat. sol. in HtO contain 0.7 gm. m acid at 15^ and 4 gms. at 50*.
« 44 44 44 44 44 QAA " h " " '* " 2 Q8 " " "
" " "CHsOH" 53.58 " m " " "
" " " " " 236.22 " p " " " (Savorro, 1914^
" 95% formic acid dissolve 2.37 gms. m acid at 20.8^. (Aachan, 1913-)
141
BENZOIC ACIDS
Mutual Solubility op Mbta and Para Oxtbbnzoic Acids and Water and
OF Parambthoxybbnzoic Acid and Water at High Temperatures, De-
termined BY THE Synthetic Method.
Meta Oxybenzoic Acid
+H,0.
fof
Melting.
xoo Gma
Mixture
78.2
9.9
90.8
20
98
30
103.2
39-8
108.8
49
119. 2
60
131-4
70
143 -4
77-9
17s -6
90.8
199.8
100
(Fbtschner and Rankin, 1910.)
Para Oxybenzoic Add
+H,0.
Cms. Acid per
xoo Cms.
Mixture.
t*of
Melting.
77
90
97.4
104.4
III. 8
120
134
154. 4
180.6
213
10
19.8
29s
40.1
SO
59-6
69.2
80
90 4
100
Para Methoxybenzoic
Acid + H,0.
Cms. Add per'
100 Cms.
Mixture.
crit. sol. t.
fof
Melting.
138.2
140
142
144
145
146
ISO
160
170
184
9
12
18
30
594
73-3
89.8
95.6
100
Readings for t^ of critical saturation obtained by cooling from t^ of melting,
are also ^ven by the authors.
Coefficients of distribution of oxybenzoic adds between water and olive oil
are given by Boeseken and Waterman (191 1) as follows:] p oxybenzoic acid,
0.6; m oxybenzoic add, 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.
MethylBINZOIC ACIDS C6H4COOH.CH.. 0, m, and p.
Solubility in Water.
(Vaubel, 1895)
f.
25
Cms. CJIiC00H.CHa per xooo Cms. Sat. Solution.
Ortho
1. 18
Meta.
0.98
Para.
0.35
NitroBENZOIC ACIDS QH4.NO1.COOH. o,'m,andp.
Solubility in Several Solvents.
(de Connick. 1894; for solubility in UK), see also Paul; Vaubel; LOwenherz; Goldsclimidt, 1898; HoUe-
man, 1898; Noyes and Sammet, 1903: Sidgwick, x9xo.)
Solvent.
f.
Cms. CJI1.NQ1.COOH per xoo cc. Solvent.
Water
IS
20
25
30
35
Methyl Alcohol lo
Ethyl Alcohol lo
" (abs.) 15
" (33VoL%) 15
It
It
tt
tt
ts
Acetone
Benzene
Carbon Disulfide
Chloroform
((
tt
tt
Ether
ligrdin
10
10
10
10
15
25
35
10
10
Ortho.
0.625
0.682 (0.645G.)
0.738(0.7790.)
0.922 (0.922G.)
1. 141 (1.054)
42.72
28.2
37.58*
0.64(11.8^)
41.5
0.294
0.012
0.455 (11^)
1.06'
1. 13
1.59*
21.58
trace
MeU.
Para.
0.238
0.0213
0.315
0.039
0.341
0.028(0.045)
• ■ •
0.477
• • •
0.0419
^^H ox
9.6
33.1 (11. 7 )
0.9
47 . 26*
19.71*
0.52
0.055
41.5
4.54
^•795, ^^
0.017(12.5**)
0.10(8.5^)
0.007
5.678
0.066
3.4St
4.7f
0.088
'
0.II4
•
6.3it
0.156
'
25.175
2.26
0.013
0
Gms. add per xoo cc. saturated aoltttion. t ~ Gms. add per xoo gms. solvent.
NitroBENZOIC ACIDS
142
Solubility of Ortho Nitrobbnzoic Acid in Water. (Noya and Sammet, 1903.)
f.
aH4N0iC00H o per Uter Sol.
V.
OHiNOaCOGH 0 per Liter SoL
MilUmols. Grams. ' ' Millimoh. Grams.
10 26.62 4-645 25 43.3 7.231
IS 31.06 5.187 30 51.6 8.616
20 36.57 6.106
Additional determinations by other investigators, in millimols CeH4N0sCOOH
o per liter at 25®, are: ±6.$ (van Maarseveen, 1898); 44.19 (Paul, 1894); 42.3
(Holleman, 1898); 43.6 (Kendall, 1911)*
Solubility op Ortho, Mbta and Para Nitrobbnzoic Acids in Water
AT High Temperatures, Determined by the Synthetic Method.
(Flaachner and RAnkin, 1910.)
0 CeH4N0iC00H+H,0. m C:aH4N0iC00H+H,0. p C«H4N0tC00H+H,0.
fof
Melting.
Gms.Add
per zooGma.
Sat. Sol.
5
9
US
30
S3. 5
65.5
76.7
83.2
88
J 95.2
100
Data for the solubility of mixtures of 0, m and ^nitrobenzoic acids in water at
24.4^ are given by Holleman (1898}.
S(x.ubility op Ortho Nitrobbnzoic Acid in Aqueous Solutions of Hydro-
chloric, Formic, Malonic and Salicylic Acids at 25^. (Kendall, 19x1 J
Gms. o
Solvent.
i* nf
Gms. Acid
t* oL' G°>^ Add
* fn
per 100 Gms.
Sat. Sol.
Melting.
Melting.
Solution- ' Sat. Sol.
M
52 crit. t.
• • •
63.2
2
118
69
5
4
... 6
143
75
9.9
4
90 7
ISO
78.
13.5
A
100 10.5
iSS
79
49-5
4
105 17
160
80
62
4
107 . 5 crit. t. 30
i6S
85
73-5
4
106 50
170
90
78.6
4
100 58.6
180
100
83.5
4
90 65.4
190
120
94
80
74
200
148
100
100
• . • 00 . 5
220
120
... 96.8
237
140.
4
100
Solveat.
HCl
«
tt
tt
tt
HCOOH
tt
Normality
oi Solvei^
0.0179
0.0357
O.I2S
0.250
0.500
0.0517
0.0998
Gms. o
OHiNOiCOOH
per Liter Sat.
Solution.
6.146
5.661
4.976
4-997
4.752
7.188
7.124
NormaUty aHiN0i.C00H
of Solvent, per Liter Sat.
CH,(COOH),
tt
tt
tt
C,H4(0H)C00H
tt
tt
O
0.0313
O.IOOI
0.2004
0.0094
0.0136
0.0162
Solution .
7.281
7.144
6.934
6.656
7.276
7.352
7.369
Sc^uBiLiTY OP Ortho Nitrobbnzoic Acid in Aqueous Solutions op
Dextrose, Sodium Chloride, and op Sodium Nitrate.
Original results in molecular quantities. (Hoffman and Langbeck, 1905).
In Dextrose.
In NaCI.
*ln NaNOs.
O.CH«OsO.(a)CeH«NOj.COOHG.Naa. G.(*)C|H4NOj.COOH G2TaN0» G.(o)CeH«NOj.COOH
|Kr 100 cc. per loo g. Solvent, per loo cc. per loo g. Solveiit. p^ loo cc. per loq g. Solvent.
At af. Atl?. Solution. At as". At 35*. Solution. ' At a^. At 3S*.
Solution.
O.O
0.36
1.80
950
20.00
0.736
0.736
0.732
0.722
0.703
1.063
1.064
1. 061
1. 051
I 030
0117
0.195
0.585
2-425
5.80
0.743
0.746
0.749
0.688
0.597
1.072
I 075
1.070
0.967
0.831
0.170
0.284
0.851
4-255
8.510
0.746
0-754
0.767
0-774
0.748
1.074
1.080
1.096
1.097
1. 047
143
NttroBINSOIO A€JM
SoLumLiTT or Omho Nitrobbnioic Acid in Aqueous Solutions or
Sodium Buttsatb, Acetatb, Formats, and Salicylatb at 264*.
(PlttBlMSoS^
Orisinal
Mols.
gUUU I^SUiti
a au Mauisi \tL
100 '^
'
GoM-NaSftk
GttB. Oitko CACOOHHOi per liter of SoHitko b :
per liter.
C^rC0ON«.
(%CXX>N«.
BCOONa.
C«il« OH-COOtlk.
0
7.8s
78s
785
7-85
OS
8.3s
8.50
8.60
8.3s
z.o
890
9IS
9 50
8.70
2
zo.o
ZO.80
II. s
9 4
3
iz.a
^^'S5
»3-5
II .0
4
12.4
MS
15.6
"5
6
IS a
• • •
• • •
• • •
Solubility of Ortho Nitrobbnzoic Acid in Sbvbral Alcohols.
(Timofeiew, 1894.)
Cms. Acid per 100 Cms.
Soivcii^
f.
CHtOH
•
0
it
22
CJBtOU
0
li
22
Solvcoft.
r.
SaLSoL Solvent.
36.2 56.6 CaHTOH o
52.2 109. I " 22
23.3 30.4 (CHs),CH.CH/)H o
42.7 745
Omt. AcM per too dm
i SaLSd.
17.7
31-2
9.6s
Solvent,
21.5
4SS
Z0.7
Freenne-point data for mixtures of 0 nitrobenzoic acid and dimethylpyrone are
given by Kendall (1914a).
Solubility of Mbta Nftrobenzoic Acid in Sbvbral Alcohols.
(nmoidew, 1894.)
SoivenL
f.
Gms. Acid
ta 100 Gms.
»•.
Gmt-Add
Sat. Sol.
per 100 Gmi
S«t.Sol.
Solvent. -^"^
Solvent.
CHiOH
0
19
41.9
53-7
73.3 C,H»OH
116 CtHTOH
ai-S
0
43-9
34.1
89.8
31.8
C>HtOH
31. S
0
57. 1
33-6
133 • I
S0.6
19
31.5
31
3«.5
4S
48
«
19
43.3
73-2
Solubility of Mbta Nitrobbnzoic Acid in Aqubous Solutions of Sodium
Acbtatb, Sodium Formatb, Sodium Monochloracbtatb and Potassium
" formatb at 25^.
(Philip and Gamer, 1909.)
In CHiCOONa. In HCOONa. In CHiClCOONa. In HCOOK.
Gms. per liter.
Gms. per Liter.
CHr
COONa.
O
Z.009
2.484
S-027
10.07
iiCiH«NO»-
COOH.
3 424
S-I44
7 932
Z2.6l
20.77
HCOONa. **cOOhP^
Gms. per Liter.
« -
Gms. per Liter.
O
0.843
2.102
4.196
8.410
3 424
4.77<^
6.380
8.616
11.90
CHiCl-
COONa.
O
I.37S
3.426
6.839
13.710
m CiHiNOr urr^it
COOH. n^^Ai*"
3.424
4.07s
4.876
5.861
7.264
O
1.025
^.563
5 -"4
mC«H4N0|.
iCOOH.
3 424
4.742
6.446
8-SSi
NitroBENZOIC ACIDS 144
Solubility op Para Nitro Benzoic Acid in Aqubous Solutions
OF Anilin and op Para Toluidin at 25^.
(LOweohen — Z. phjak. Chem. 3& joSt 'gS*)
In Anilin. In />-Toluidin.
G. Mob. per Liter. Gnu. per liter. G. Mols.j)er liter. Gmt. per liter.
CO 0.00164 0.0 0.274 0.0 0.09164 0.0 0.274
o.oi 0.00841 0.91 1.406 o.oi o.oioo 1. 071 1. 671
0.02 001379 1.82 2.304 0.02 0.0174 2.142 2.902
004 002172 3.64 3.629 0.03 0.0245 3.213 4097
008 0.0347 7.29 5.798
1000 cc. of sat. solution of pira nitrobenzoic acid in aqueous i normal sodium
para nitrobenzoate contain 0.0046 gm. mols. » 0.768 gm. ^CftH4N0sC00H at
25*. (Sidgwkk, 1910.)
Solubility of Para Nitrobbnzoic Acid in Several Alcohols.
Sohroit.
CH*OH
it
CiHtOH
«
CTSmofeieii
r. x«94)
f.
Gms.Acid]
;>eriooGBis.
^SaIvmi*
a*
Sat. Sol.
Solvent. '
.MfftVCIIb.
V .
SAt.SoL
Solvent. '
18.5
3-45
3. 57
CtHiOH
31
3.22
332
21
3.7s
3-90
CiHjOH
i8S
2.12
2.17
18. s
3-25
3-36
((
19s
1.85
1.90
19s
316
3.26
€t
31
2.29
2.34
DinitroBENZOIC ACIDS CcH,(NOi),COOH. 1.3.5 and 1.2.4.
S(H<UBILITY of 3.5 AND OF 2.4 DlNTTROBENZOIC ACIDS IN AqUBOUS
Solutions of Sodium Acetate at 25^.
(Philip and Gamer, 1909.)
Gms. per xoe oc. Sat. SoL Gnu. per zoo cc. Sat. Sol.
CHiCOONa. j.5aHa(N0i),C00H. CHtCOONa. 2.4C«Ha(N0i),C00H.
o 0.1314 o 0.0572
0.0976 0.3392 0.0976 0.2056
0.2428 0.6720 0.2428 0.3434
0.4846 I. 201 0.4846 0.5023
e.9718 2. 115 0.9718 0.7440
Data for the solubility of 1.3.5 dinitrobenzoic acid in water and aqueous
solutions of KCl, NaCl, KNOi and NaNOi, 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.
(Flaichaer and Rankin, 19x0.)
r M Gms. Add pa*
* * zoo Gmt. Sd.
160 90.9
180 95
200 99
206 xoo
M Gmt. Add per
^* zoo Gmi. Sol
f.
Gme.Acid
zoo Gms. 1
123.8 critt. ...
123
66.5
113 4.4
125
72.7
120 9.3
130
79-3
121 14-5
140
«S-7
122 40
150
89
145 NitroBENZOIC ACIDS
Solubility of Nitrobromobbnzoic Acids and op Nitrochlorobbnzoic
Acids in Water at 25**.
(HoUemui, 19x0.)
C6H,C00H.NQi.Br 1.2.3 0.033 CsHaCOOH-NOiCl 1.2.3 0.047
CJEI,COOH.NQj.Br 1.2.S 0.741 CfH,COOH.NQi.Cl 1.2.5 0.967
Holletnan also gives data for the solubility of various mi3ctures of the above
two bromo compounds and of the two chloro compounds aiid* uses the results for
estimating the quantity of each in an unknown mixture.
Dinitro p oxyBENZOIC ACID CaitOH(NOi)tCOOH.
S(h<ubility of Mixturbs of Dinitro Para Oxybbnzoic Acid and Othbr
Compounds in Absolute Ethyl Alcohch. at 29.6^
(Morgensteni. 19x1 )
Dinitro P Oxybeozoic Dinitro p Oxybenzoic Dinitro P Oxybenzoic
Add + Phenanthrene. Acid 4* Fluorene. Add + Retene.
Solid
Phase.
Add
M
Cms. per 100 gms.
Solid Phaae.
Sat.
100 Cms.
Sol.
SoUd
100 Gma.
.SoL
Add.
Pheoaa-
thnne.
And.
Fluorene.
Phase.
Add.
Retene.
2.0483
0.1333
Add
2.0440
0.1232
Add
2.0232
0
2.0776
0.2796
u
2.0823
0.3484
u
2.0484
0.1236
2.X249
0.5267
i(
2.1045
0.4824
u
2.0933
0.3446
2 . 3195
1.0311
11
2.1744
0.8960
it
2.1276
0.5162
2.2883
I. 4310
i<
2.2618
X.4308
n
2.2346
X.0489
X.2171
6.0092
Phenanthiene
1.0490
3.8618
Flttoiene
2.3034
1.3634
0.8681
S.8300
i<
0.8004
3-7566
«
1.9664
3.3698
0.6017
5.6890
<(
0.5620
3-6532
II
0.7830
3-0032
0.3487
5-5619
If
0.3900
3.581I
(1
0.5597
2.9331
0.2157
5.4890
(1
O.2113
3.5024
(1
0.2740
2.8466
0
5.3781
n
0
3.4115
II
0
2 . 2795
BENZOIC A19HTDBIDE
(C«H,CO),0.
<l
11
II
II
Retene
II
II
II
II
Freezing-point data are given for mixtures of benzoic anhydride and sulfuric
add by Ivendall and Carpenter (1914).
BENZOIN (Benzoyl phenyl carbinol) CcHtCH(OH)COC«Hi.
'S(x«uBiLiTY OB Benzoin in Watbr, Pyridinb and Aqueous 50% Pyridine
AT 20-25'*.
(Ddin. 1917.)
Solvent.' ^™** BenMin pa zoo
*~'^^"** gma. Solvent.
Water o 03
Aq. 50 % Pyridine 6.63
Pyridine 20.20
100 gras. 95% formic add dissolve 3.06 gms. benzoin at I8.5^ (Ascfaan, xgzs-)
Freezing-point data (solubilities, see footnote, p. i) are given by Vanstone
(i9i3)ff for mixture of benzoin and each of the follo¥ring compounds:
Dibenzyl, beozylaniline, benzylideneaniline and hydrazobenzene.
BENZOPHENONE
146
BXHZOPHXHOHX (CeH.),CO.
Solubility in Aqueous Alcohol and in other Solvents.
(Deniea — ComiA. rend. lacH 7»9» '00; Bdl — J. Phspsic. Chem. 9, 550, '05.)
In Aqueotis Alcohol at 40^.
(BeU.)
Wt.% Cms. (CeH«)aCO
Alcohol per 100 Cms.
bSolTeat. Solvent. Sdution.
40
45
SO
55
60
65
5
8
II
16
28
1.9
4.8
9.9
13 -8
22.6
Wt.%
Alcobol
inSohtot.
67 -5
70
71
72
72-5
73
Gins. (CA)sC0
per 100 Gms.
Solvent.
39
56
67
90
los
156
SolutioiL.
28.1
35-9
39 a
47-4
Sia
61.0
In Aqueous Alcohol and other Solvents.
(Deirien.)
SoIvenL
f.
Gms.
(aH«)tCO
per xoooc.
Solvent.
Solvent.
Gms.
(CiHOtCO
per xoooc.
Solvent.
97% Ethyl Alcohol 17
8s cc. gy% Alcohol + 15 cc. HjO 17
80 " " + 20 " 17
75 " " + 26 " 17
Methyl Alcohol (pure) 9 . 8
It tt it -g
Acetic Ether (pure) 9.6
Carbon Disulfide 16. i
13.5 Ethyl Ether (rectified) 12.7
3.8 Benzene
2 . 2 Xylene
1.3 Nitro Benzene
II Chloroform (com.)
14.3 Bromoform
19 . 2 Toluene
66.6 Ligr5ine
17
17.6
iS-8
16.5
173
17.2
14.6
17
76
38
ss
55
33
55
6
4
8
5
3
5
7
Determinations made by means of the Pulfrich refractometer (Osaka, IQ03-8),
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 TiMMERMANS (1907).
In Aq. 7i.i
(Sat. t
In Aa. 36.51% CHiOH
(Sat. t = 65.3).
fof
Sat
75-4
81. 1
85.3
88.1
Gms. (aHt)sCO
per xoo Gms. Sat.
Sol.
0.685
1.06
1. 41
1.67
fof
Sat.
26.1
293
39-5
S5-5
82.6
^% CeHjOH
= 20.6).
In Aq. 39.
(Sat.
4% CHtCOOH
t » -2.3).
Gms. (aH>)tCO
per xoo Gms.
Sat. Sol.
f.of
Sat
Gms. (CeHc)tCO
per xoo Gms.
Sat Sol.
0.96
6.1
0-439
1.77
18.5
1. 13
4.06
28.9
1. 71
7.82
44
2.66
16.82
61.6
3 92
75-2
5.09
Solubility data for mixtures of benzophenone and resorcinol and for benzo-
phenone and pjnrocatechinol, determined by the freezing-point method, are given
by Freundlich and Posniak (1912). Similar data for mixtures of benzophenone
and thymol are given b^ Pawlewsla (1893). Results for mixtures of benzophenone
and sulfuric acid are given by Kendall and Carpenter (i9i4)«
BENZOYL GHLORIDS, BENZOYL tetia 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 I forms of benzoyl
tetrahydroquinaldine, by Adrian! (1900).
U7
CaiiCH,.NH,.Ha,
100 gms. HiO dissolve 50.6 gms. of the compound at 25**. (P«ddk aad Tonwr, 19130
DiBBHZTLAMDIB HTDBOGHLOBIDB (CACHOtNH.HCl.
100 gms. HsO dissolve 2.17 gms. of the compound at 2^**. (Poddk aad l>uner, x^i^O
100 gms. chlorofonn dissolve 0.37 gm. of the compound at 2$\
TriBBNZTLAMIHB HTDBOGHLOBIDB (CJitCHOiN.HCt.
100 gms. H/) dissolve 0.61 gm. of the compound at 25^ (Feddk and Tomer, 1913^
100 gms. chloroform dissolve 1 1 41 gms. of the compound at 25^ **
EHBBNZYL aHtCHs.CJi»CH>, BBNZTLAIOLINB CaisCHt.NHC«H«.
Solubility Data, Dbtbrminbd by thb Frsbzing-point Mbthod (see
footnote, p. i), Arb Givsu for the Following Mixtures:
Dibenzyl+ Stflbene
+ Benzylphenol
+ Hydrobenzene
4-ToIane
Beazylaniline + Dibenzyl
ff
«
<i
(Bnui, 1898: Pasal and Nomand, I9os0
(Pascal and Nomand, X9i3*)
u
l<
+ Stilbene
M «
«
+ Benzylphend
M «
u
4- Hvdrazobenzene ** "
u
1 * ^J ^»B» ^•^•^^•^^^••iMF^""-"
+ ToIane
•
M «
NitroBENZTL CHLOBIDE p C«HtCHNOs.Cl.
Solubility in Sbvbral Solvents at 25^ (v. Halbaa. 19x30
<
^ms. p CiHiCHJfOia
Gna. # OHiCRNQ^a
Solvent.
per zoo
Gms.
Solvent.
per 100
Cms.
Solvent.
Sat.Sol.
Solvent
Sat. Sol.
Methyl Alcohol
8.87
8. IS
Nitrobenzene
57-8
36 -4
Ethyl Alcohol
7.10
6.63
Ethylacetate
57. 8
36.4
Propyl Alcohol
S-70
539
Ethylbenzoate
43.3
30.2
Amyl Alcohol
4.88
4.6s
Ethyhiitrite
SI. a
53-9
Butyl Alcohol
ai-S
17.7
Isoamylbromide
"•S
10.4
Acetic Add
18. 1
iS-3
Brombenzene
3a
24.2
Acetone
107
SI. 7
Chlorofonn
47.6
32.3
Acetq>henone
63.1
38.7
Carbon Tetrachloride 6 . 05
5 69
Paraldehyde
24.9
19.9
Benzylchloride
453
31.2
Ether
23.1
18.8
a Bromnaphthaline
3«.7
23.4
Acetonitrile
96.6
49.1
liHexane
X.30
X.28
Nitromethane
68.8
40.8
Isopentane
0.49
0.49
0 Nitrotoluene
SI. I
33.8
Benzene
69.7
37.4
Data for the lowering of freezing-point are given by HoUeman (1914) for mixtures
of 0 and p nitro benzylchloride.
HTDBAZnn CeH«CH,.NH.C<HtCHsNH.
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;.
ChloronitroBSNZTLIDINISC«H<C:NOt.Cl. BINZTLXDINI NAPHTHAIr-
AMINX8 OHtCHiNCiaHr.
Data for thb Lowering op thb Frbbzing-points (solubilities, see foot-
note, p. i) Arb Givbn for thb Following Mixtures.
0 Chloronitrobenzylidene + m Chloronitrobenzylidene (HoUeman, 19x4-)
P " +m
p " +0 " «
a Benzylidene naphthalamine+^ Benzylidene naphthalamine (Pascal and Nonnand, 'xsO
BEBTLLIUM ACETATB (basic) Be«0(CH,C00)6.
100 gms. chloroform dissolve 33.3 gms. Be40(CH|CC)0)f at I8^ (Wiith, 19x4^
BEB7LLIUM FLUOBIDS 148
«
BEBTLLIUM Potassium FLUORIDE, etc
Solubility in Water and in Acetic Acm Solutions.
(Marignac; Sestini, 1890.)
Cms. Anhydrous Salt
Salt Fonnula. Sotvent. per 100 Cms. Solveat.
At ao". At xoo*.
Beryllium potassium fluoride BeFs.KF Water 2.0 5.2
sodium " BeF,.NaF " 1.4 2.8
" hydroxide Bc(OH)f Water + CQi sat 0.0185 (BeO)...
phosphate Bei(P04)i.6HiO 2% CHiCOOH 0.055
10% " 0.1725
i( II II
BERYLLIUM HYDROZIDK Be(OH)s.
Solubility in Aqueous Solutions op Sodium Hydroxide.
(Rubenbauer — Z. aiuxg. Chem. 30 534, ^a.)
Moist Be(OH), used, solutions shaken 5 hours, temperature pro1>
abiy about 20**.
Molecular
Per ao cc. Solution. Dilutioa Cms, per loo cc. Solution.
Cms. Na. Gnii. Be: ^^^ NaOH. Be(OH)|.
03358 0.0358 1.37 a. 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 Hybroxidb at Different Temperatures.
(Habar and Oordt, 1904.)
Nomial^of Gm. BeO per Ijter Sat. Sol, at:
Aq.NaOH. ^^^^o ^^^o ^^o
0.5 0.060 0.080 0.080
1 0.170 0.230 0.290
2 0.570 0.900 X.020
BERYLLIUM OXALATE BeCOisHsO.
100 gms. water dissolve 63.2 gms, BeCi04.3H|0 at 25^ (Wirth, 19x4.)
•^ cm oxalic acid " 75.92 " " '^
o.in sulfuric " " 72.65 "
1.0 n " " •• 52.8 "
BERYLLIUM PAUOTATE and Salts of Other Fatty Acids.
Solubilities in Ethyl and Methyl Alcohols at 25^ Cjaoobaon and Holmes, 1916.)
Cms. of Each Salt (Determined Sepantebr) per too Gms. Solvent.
Solvent. / ^ %
Be Palmitate. Be Steamte. Be Lauxate. Be Myristate.
Ethyl Alcohol 0.004 ... 0.004 0.004
Methyl Alcohol 0.042 0.040 0.050 0.047
BERYLLIUM SULFATE BeSOi.eHsO.
Solubility in Water. (Levi, Maivano, 1906.)
^:^ °°1c?g£;.'*' s.«d ^-m '"^JfStr Solid
31 11.18 52.23 34.32 BeS04.6HtO 95.4 6.44 90.63 47.55 BcSO«4RO
50 9.6a 60.67 37-77 *' 107-2 5-o6 1x5.3 53-58
72.2 7.79 74.94 42.85 " III 4.55 12^.3 56.19
77-4 7-13 81.87 45-OI " 80 6.80 84.76 45.87 BoSOa^B^
72.2 7.79 74.94 42.85 " III 4.55 12^.3 56.19
6.80
30 13-33 4378 30-45 BeS044H|0 91.4 5.9^ 97.77 49.42
40 12.49 46.74 31.85 '* 105 4.93 118.4 54.21
68 9.42 61.95 38.27 *' xxp 3.91 X49.3 59.88
8S 7'6S 76.30 43.28 •'
If
««
149
BERYLLIUM SULFATE
Solubility of Beryllium Sulfate in Aqueous Sulfuric Acid at 25*
(Wirth, I9ia-i3.)
Cms. HsSOc
Gnw.BeSO«
Cms. HsSOi
Gms. BeSOi
pa* zoo Cms.
per 100 Cms.
Solid Phase.
per zoo Gms.
per xoo Gms.
Solid Phase.
Solvent.
Sat. Sol.
Solvent.
Sat. Sol.
0
8.212
BeS04.6H20
45. SI
6.628
BeS04.6H20
S-23
8.429
50.63
S.438
BeS04.4H20
. 9-6i
7-944
56.59
3.640
«
18.70
6.603
63.24
2.244
tt
34
5-631
65.24
2.128
€t
40.3s
5-773
73-64
2.18s
ii
Freezing-point data for mixtures of beryllium sulfate and potassium sulfate are
given by urahmann (1913).
j^ERTLLIUM MetaVANADATE Be(VQi),.4H,0.
100 gms. HsO dissolve o.i gm. of the salt at 25^
BETAINE (Trimethyl glycocoU) C»HuOiN.HsO.
(Brinton, i9z6.)
Solubility of Anhydrous Betainb in Water and Alcohols.
(Stoltzenbeig, 1914)
(Figures read from the author's curves.)
f.
' Cms. CiHuOiK per
100 Gms.
f.
Gnu. CiHuOiK per
100 Gms.
:HiO.
CH/>H.
CAOri.
MA
CHK>H.
C»H»0H.
— 10
134
38
S
50
197
70
16
0
140
43
6
60
215
75
18. s
+10
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.
SoLUBn.iTY OF Each, Separately, in Water.
(Stoltzenbeig, 1914-)
Grams per xoo Grains HsO.
.
f.
OHuOiN.
OHuOiN.
CsHuOiN.
aHuOiN.
CsHuOiN.
CtHuOiN.
CiHuOiN.
hq.
HBr.
HT.
HsS0«.Hs0.
H.P04.
HMnOk
HAuCU.
— 10
38
28
35
67
35
1-5
1-3
0
44
39
66
86
45
1-75
I-S
+10
52
52
98
107
58
2.5
2
20
60
65
130
132
73
5
3
30
70
79
162
164
91
9
4-5
40
81
94
198
203
112
16
6
50
93
no
231
250
135
, .^°
8
60
106
127
269
306
160
(55°) 48
"5
70
120
144
304
■ • •
190
...
15
80
135
162
(75^) 321
• • •
223
...
18
90
151
183
• • •
• • •
...
...
23
100
169
206
• • •
• • •
...
...
• • •
Data are also given by Stoltzenberg for the following basic salts of betaine
(C.HiiO,N),HCl.H,0, (C,HuOiN)2.HBr. (C,HuOiN),HI. (C,HiiOiN),H,S04 and
{CfHiiO,N)2HAuCl4.H,0.
BETOL OS-Naphthylsalicylate) /9C7H«0,.CioH7.
Freezing-point data*including super solubility curves, are given for mixtures of
betol and salol by Miers and Isaac, 1907.
BISMUTH 150
BISMUTH Bi.
Reciprocal Solubilities, Determined bt the Method op Lowering of
TusioN-poiNT (see footnote, p. i), Are Given for the Following Mixtures:
Bismuth + Bromine CBgpak, 1908.)
+ Chlorine
** + Iodine (Amadori and Becarelli, 1913.)
" + Sulfur (Aten, 1905; Palabon, 1904.)
Mutual Solubility of Bismuth and Zinc. (Spring and RonMtnofi. 1906.)
t* Upper Layrr. Loirer lairer. ^ Upper Layci. Lower lajFer.
%Bi. %Zn. %Bi. %Za. %Bi. %Zn. %Bi. %Zn.'
266 86 14 584 80 20 10 90
419 3 97 650 77 23 IS 8s
475 84 16 5 9S 750 70 30 27 73
810-820 (crit temp.)
BISMUTH CHLOBIDB. BiGt. BSMUTH OxyCRLOBIDE BiOCl.HtO.
SCH^UBILITY IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID.
Results at 25®. (N<ve> and Hall, 1917.) Results at 30®. Gacobs. X9I7-)
<U» Sol
Gms. Atoms per xooo Gna. H^.
Gms. per 100 Gms. Sat.
Solution.
A.
SnlM Phase.
oac. ooi.
CI.
Bi. H(-Cl-3Bi).
BiiQi.
HCI.
1.002
0.3477
0.00130
0.3438
0.60
2.40
BXX3.aO
1.007
0.4350
0.00376
0.4237
5.35
5-69
M
1. 010
0.5221
0.00869
0.4960
8.17
8.47
M
1. 013
0.6244
0.01767
0.5714
8.70
8-93
«
1. 018
0.737s
0.03138
0.6434
14.52
13.02
M
I.02S
0.8824
0.05338
0.7223
18.60
iS-8o
M
1.036
1.0760
0.08937
0.8079
30.10
21.7
M
1.044
1.2277
O.II77
0.8746
36.95
25-4
a
1. 061
I 5321
O.181O
0.9891
54.70
31S
«
1.083
I. 9021
0.2657
1.105
56
328
Bioa
IIS7
3.186s
0.5685
1. 481
58.5
33
BiCk.2lU)
1.237
4.5056
0.9022
1.799
56.6
33-8
•• +BiCb
1.288
5325
1. 100
2.025
56.25
34-9
BiCla
1.329
6.066
1. 317
2.115
55.9
35-9
BiCli.Ha
S0LUBILIT1
r OF Bismuth Chloride
IN Several Scv^vents.
CmIm...
^&
f.
Gms. BiCb per xoo.
boiveiu.
cc. Solvent.
Gms. Solvent.
Authority.
Acetone
18^
... 17.9 (rfi8=0.
>9I94)(NMimiim, 1904, '05.)
Ethyl Acetate
18^
• • • X •
66((2u=o,
.9Io6)(Nsuiiiaiiii, 1910).
Anhydrous Hydrazine ord. temp. 32 ... (Wdsh and Broderaoo. 1915.)
100 gms. 95% formic acid dissolve 0.05 gm. bismuth oxychloride (BiOCI) at
19.8^. (Aschan, 1913.)
Freezing-point data are given for BiCU+CuCl, BiCU+FeCli, BiCU-f PbCU,
BiCU+PbBrj and BiCU+2nCli by Herrmann (191 1) and for BiCU+TlCl by
Scarpa (1912).
BUMUTH CrnUkTE (CHi),C(OH)(COO)iBi. BISinTTH Ammonium
CITRATE.
Solubility of Each in Water and in Aqueous Ethyl Alcohol at 25^. (Seidell, 'xa)
Gnu» GHgHpcr ^."^gS^^S Gms COIgH per Sil^^^^oo rf. Sat. Sol.
xoo Gms SdveDt. "^ ^ ^*^ ^~** xoo Gms. Solvent. GnaTSoL sST
o o.oii o 22.25 1.25
51 0.041 51. 1.34 0.92
91.4 0.065 91.4 None 0.81
151 bisbhtth htdbozids
bismuth htdbozide bi(oh),.
SCX.UBILITY OF BiSMUTH HyDROXTOB IN AqUBOUS SOLUTIONS OF SODIUlf
AND Potassium Hydroxides at 20** and at 100**.
(Moser, 1909.)
Gmt. KOH G"«. Disaolved Bi(QH)» per Liter att q^^ NaOH ^°"' J^^*»olv«* Bi(0H)» per Liter at:
P«^^- ' ^, ' '^, ' per' Liter. '—^ ' ^^^
28 o 0.188 20 o 0.188
50 trace 0.249 40 trace (0.0014)* 0.249
112 0.037 0.373 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(0H)8 was converted into BiO(OH).
Solubility of Bismuth Hydroxide in Aqueous Solutions of Potassium
Chloride and op Potassium Bromide at yf,
(Herz and Bulla. 1909.)
(An excess of bismuth hydroxide, prepared according to Moses and having the
composition corresponding to BiO.Orl, was shaken 2-3 weeks at 30^ with aqueous
KCI and KBr. The analyses of the sat. solutions are expressed m terms 01 milli-
mols KOH and KCI or KBr. They have been calculated for the following
table to gms. BiO.OH and KCI or KBr.)
- . ^ Gms. per 100 cc. Sat. Sol. „ , Gms. per 100 oc. Sat. Sol.
^^'' ' BiCOH. • KCT ^^'- 'Bi0.0H. ' KbT
2nKCl 3. 759 i3-7S in KBr 8.555 7-67
3»KC1 S-74S 20.71 2nKBr 17. 785 15.02
BISMUTH IODIDE Bil,.
100 gms. absolute alcohol dissolve 3.5 gms. Bils at 20^. (Gott and Muir, 1888.)
100 gms. methylene iodide, CH2l2, dissolve 0.15 gm. Bilt at 12''. (Retgers, 1895.)
BISMUTH NITRATE Bi(N0,),.5H,0.
100 gms. acetone dissolve 48.66 gms. Bi(NC)»)|.5H|0 at o**, and 41.7 gms. at
19 • (von Laszcqmski, 1894.)
Solubility of Bismuth Nitrate in Aqueous Nitric Acid and in Aqueous
Nitric Acid Containing Acetone, at Ordinary Temperature.
(Dabrisaay, 19x1.)
**~»- ^i^iS'Sf^ Solid Ph«e.
0.932 »HNOi
86.86
Bi(NO,),.sH,0
0.922" " + 6.66% Acetone
85 SI
U
0.922 " " +13.33% "
81.96
tt
2.3 " "
80.37
It
2.3 " " +16.66% "
74-47
u
Solubility op Double Nitrates op Bismuth and Magnesium, Nickel,
Cobalt, Zinc and Manganese in Conc. HNOi at 16**.
Gantsch, 1912.)
(di6 of HNOi = 1.325, 100 cc. of this acid contained 51.59 gms. HNOi.)
Gms. Hydratcd Gms. Hydrated
Doable Salt. Salt per 100 cc. Double Salt. Salt per zoo cc
Sat. Solution. Sat. Solution.
Bi2Mg,(NQ8)i2.24H20 41 69 Bi2Zn3(NO,)i2. 241^0 57 . 51
BiJNi,(NQ,)i2.24H,0 46.20 - Bi2Mn3(NO,)u.24H20 65.77
Bi«Co,(N08)i2.24HjO 54. 67
BISMUTH OZIDl
152
BISMXTTH OXIDE Bi,0,.
Solubility of Bismuth Oxide in Aqueous Nitric Acid at 20^,
(Rutten and van Bemmelen, 1902.)
Pment in Shaker
Flask.
Ptf I port BisQi.
jNjOs.ioHsO.
Gms. per too Cms.
Solution.
Mols. per 100 Mob. H3O.
BifOj
0.321
6.37
18.74
31.48
32.93
24.4 parts HjjO
3.2 parts H,0
Dilute HNO,
Dilute HNO,
Dilute HNO, -
6.13% NA
6.816% N,0, 32.67
24.0% N,0, 24.16
51.0% N,0, 11.66
70.0% N,0, 20.76
27.85
Anyhdrous HNO, 8.56
Bi,0,+ " 4.05
0.963
7.17
15.9
23-7
24.83
24.70
28.25
46.62
53.75
51.02
68.28
74.90
BiaOa
o 126
2.844
10.50
27.2
30.15
29.70
19.65
10.81
33.51
51.0
1435
7.45
1. 61
13.82
38.65
83.8
Solid
Phase.
97.97
96.57
98.76
186.23
355.87
403.0
492.0
592.9
J : "is } Bi,0, JJ,0, jH,0
r . 4 <> / BiflO|.N|(X JlgO and
'• 3.2 t Bi,Oi.3NsO,.ioHiO
x: 3.2'
x':i7!2 BitOi3N.O,.ioH,0
x:io.6.
. ,,orBi,0,.3N,0,.ioH.O
'• /-^ 1 BigO,.3Ng08.3H,0
J;79:sl^»^-^^-A^
and
Results are also given for 9®, 30®, and 65®.
BISMUTH TriPHBNYL Bi(CeHt)i.
Fusion-point data (see footnote, p. i) are given for mixtures of bismuth
triphenyl and mercury diphenyl by C!ambi (1912).
BISMUTH SALICYLATE (basic, 64% BisOi).
Solubility in Aqueous Solutions of Ethyl Alcohol at 25**.
(Seidell, 1910.)
Gms.GHiOHper
100 Gms. Solvent.
O
20
40
60
Cms. Salt per
xoo Gms. Sat. SoL
O.OIO
0.015
0.022
0.036
Gms CiHtOHper
100 Gms. Solvent.
80
90
92.3
100
Gms. Salt per
xoo Gms. Sat. Sol.
0.065
0.095
0.105
0.160
BISMUTH SELENIDE BisSe,.
Fusion-point data (see footnote, p. i) are given for mixtures of bismuth sele-
nide and silver selenide by Pelabon (1908).
BISMUTH SULFIDE Bi,S,.
I liter HtO dissolves 0.00018 gm. BisSi at 18^.
(Weigcl, 1906; see also Bruner and Zawadski, 191 2.)
SCX.UBILITY OF BiSMUTH SULFIDE IN AqUEOUS AlKALI SULFIDE SOLUTIONS AT 25**.
(Knox, 1909 )
Solvent.
0.5 n NaaS
i.on
1.5 n
0.5 n K2S
I n
i.S»
it
ii
Gms. BbSt per
100 cc. Sat.
Solution.
0.0040
0.0238
0.1023
0.0043
0.0337
0.0639
Solvent.
0.5 nNaaS+inNaOH
I nNajS+itjNaOH
0.5 «K2S +inKOH
I wKaS+inKOH
1.25 «KaS +1.25 «KOH
Gms. BisSs per
100 cc. Sat.
Solution.
0.0185
0.0838
0.0240
o . 1 230
0.2354
Freezing-point data (see footnote, p. i) are given for mixtures of bismuth
sulfide and bismuth telluride by Amadori (1915).
BORAX, see sodium tetraborate, p. 629.
153 BOBIC ACm
BORIC AC ID HtBO,.
Solubility of Boric Acm in Water.
(Nasini and Ageno, 1909.)
^ Gms. HsBOki
*^' loo Gms. Sat.
per
SoL
r.
Gms. HiBOk per
100 Gma. Sat. Sol.
f .
Gms.HiBQi]
100 Gms. Sat
— o.76Eutec 2.27
30
6.30
80
19. II
0 2.59
40
8.02
90
23 30
+10 3-45
50
10.3s
100
28.7
20 4.8
60
12.90
IIO
38.7
25 S'S
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 op Boric Acid in Aqueous Solutions op Hydrochloric.
Sulphuric, and Nitric Acids at 26®.
(Herz — Z. anorg. Cbem. 33* 355, 34, 205, '03.)
Normality of
tlieHaS04,Ha
or HNOt.
Normality of
Dissolved
B(OH),.
Gms. Stroos Add
per 100 cc.
Solutioa.
Gms. B(OH)s per xoo cc.
, *
la HQ. In H^O«.
Sohitkn.
InHNOt.
0
0.91
0
5-64
5 64
S-64
0.5
0.78
S
4.0
4-2S
4SO
I.O
0.71
10
3-2
3-6
3-9
2.0
0.58
IS
2. 45
30
3-3S
30
049
20
1.8
2-5
a.9
4.0
041
25
■ • •
20
a 55
SO
035
30
• • •
i-SS
3.1
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 op Electrolytes
AT 25°.
(Bogdan — Ann. Sdent. Univ. Jaasy, a, 47, 'oa-*o3.)
Gms. Electro- Grams H«BOb per xoo Gms. HsO in Aq. Sdutioos of:
lyte per 100 / -^— — ■ — .^
Gms.H,0. NaQ. KQ. NaNOi. KNOj. NajSO.. KjSOi.
* o 5-75 S-7S S-7S S-7S 5-75 S-7S
lo 5-75 S-8o 5.78 5.81 5.88 5.92
20 5-74 S-S6 S-8i 5-88 6.00 6.10
40 S-72 5-98 5-87 6.04 6.33 6.50
60 5.72 6.12 5.9s 6.20 6.70 6.92
80 5.71 6.29 6.02 6.37 7.10 7.40
Interpolated from the original.
BOBIC ACID
154
Solubility of Boric Acid in Aqueous Solutions of Hydrochloric Acid
AND OF Alkali Chlorides at 25"*. (Hen. 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.)
Gms. HsBOi Diaaolved per loo cc. Sat Sol. in Aq.:
HO.
KCl.
Gms. HQ or Alkali
Chloride per zoo cc.
Sat. Sol.
O
2
4 .
6
8
10
IS
20
30
The System Boric Acid, Acetic Acid and Water at 30®. (Dukeiaki. xgog.)
(The sat. solutions^and residues were analyzed by titrating total acidity with
o.i » NaOH and the acetic acid alone by an lodometric method.)
5
4
4
3
3
3
59
92
36
88
50
IS
uo.
559
5.20
4.8s
4. 45
4.07
3-75
3
Naa.
59
40
30
20
IS
10
07
5
S
5
S
5
S
5
RbCl.
559
5.60
5.62
567
5-72
5-77
5-90
6.10
6.55
5
5
S
5
S
6
6
6
59
67
75
85
90
25
50
Gms. per loo Gms.
£S
Sol.
BiOs.
3. 55
3.18
2.98
2.34
1.98
1.47
1. 12
(CH«CO)*0.
• • •
7.78
16.44
28.96
41.06
52.63
67.76
SoUd
Phaae.
B(OH)a
«4
Gms.
xoo Gms.
t. Sol.
4<
<<
<l
Solid
- Phase. <•
BiO». (CHjC0)«0.
1. 01 73.96 B(OH)«
0.54 80.67
0.45 84.55 "+<^)
0.39 84.65
0.41 84.48
0.46 84.44
0.50 84.51
Gms. per loo Gms.
.per
Sat.
Sol.
SoUd Phase.
II
«
<f
(i
Solubility of Boric Acid in Aqueous Solutions of:
Acetic Acid at 26^. (Herz, 1903a.) Acetone at 20
Gms. per loo cc. Solutioa.
CHjCOOH
BiOi. (CHiCO)i0.
4.98 82.13 B*Oi.2(CHiCO)iO
5.13 84.60
5.41 85.68
4.82 88.74 B«Qi.3(CHiC0)^
4.71 89.98
4.06 92.68
3 10 95 76
II
l(
II
u
II
Normality of Solutions.
CUsCOOH. B(OH^
O
I
2
4
6
091
0.82
0.65
042
Q-2S
o
S
ic
20
30
B(OH)s.
5 64
4-7
4.2
30
2.0
cc. Acetone
per 100 cc.
Solvent.
(Herz and Knoch, 1904.)
B(OH)» per 100 cc. Soiution.
Millimols. Grams^
O
20
30
40
SO
60
70
80
100
79 15
81.71
83-35
82.72
81.62
76.40
67.62
55-05
8.06
4
5
5
5
5
4
4
3
o
91
07
17
13
06
74
19
41
50
SCO^UBILITY OF BORIC AciD IN AqUEOUS SOLUTIONS OF UrSA, AcBTONB,
AND OF Propyl Alcobol at 25° (Bogdan.)
Grams of
CX>(NHi)a,(CHa)jCO
Gms. HsBQji per 100 g. HsO in Aq.
Soltttioos of:
orof CiHTOHner
xoo Gms. HgO.
CO(NH2)s
A
(CH^)lCO.
CAOH.
0
5-75
S-7S
S-75
10
5-84
5 84
r-So
20
5-93
5-93
S-»S
40
6.13
6.13
5-94
60
6.31
6.39
6 03
155
BORIC Acm
Solubility of Boric Acm 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. Gm8.H^B0k Solvent. Gms-HtBOb Solvent. ^ _ ^ Gms.HiBOi
pet xoooc
Sat-SoL
0.9691
0.9340
0.9185
0.9019
0.8842
0.7960 zoo
Wt. % perioocc.
CHtO:
SO
S8
66
Gms.HtB0b
per 100 cc.
Sat. Sol.
^V OHiofi.
5.55 0.9714 20.2 S.14
6.27 0.9350 42.3 4.96
6.81 0.8789 67.3 4.52
7.20 0.8576 76.2 4.34
8.10 0.8198 91. Z 5.54
Z7.99* 0.8089 95 6.85
0.7947 100 9.47t
^-o.8904.
Wt. %
"Y" OHiOH.
0.9043 50.83
0.8231 79.41
0.8133 95.5
0.8010 100
'•ff of
_ T_ , perioocc.
Sat. Sol. Sat. Sol.
0.9193
0.8570
0.8466
0.8297
3 99
2.83
3.58
5.96
t d« - 0.8553.
In Aq. i Butyl Alcohol.
In Aq. i Amyl Alcohol.
Solvent.
0.9923
0.9853
0.985s
0.8173
0.8133
0.8081
0.7984
Mol. %
CAOH.
0.70
2. IS
2.18
714
77.1
85.6
zoo
^•.of
Sat. SoL
Z.0124
Z.0038
Z.0046
0.835Z
0.8220
0^8195
0.8172
Cms. HsBOi
per 100 oc
Sat. Sol.
S.48
S'32
2
2. IS
2.6z
430
HjO sat. with amyl alcohoL
Solvent.
o
o
o
o
o
o
o
•9943
.9936
•9931
.8232
.8183
.8142
.8068
Mol. %
OHuOH.
0.448
0.520
0.52s*
67 . 26t
75 54
83.40
zoo
tf^of Gms.H^B0)i
• per xoo cc.
Sat. SoL Sat. SoL
Z.OZ32
Z.OZ25
Z.OZ23
0.8290
0.8253
0.8223
0.8220
t "■ Amyl akohd sat. with fUO.
S.48
S-46
546
Z.60
Z.69
Z.98
3S4
One liter HiO saturated with amyl alcohol dissolves 55.5 gms. HtBOi at 15^.
(Auerbach, 1903.)
Solubility of Boric Acm in Aqueous S(x.utions of Ethyl
Alcohol at 15° and at 25®.
(SddeU, 1908.)
Results at 15*". Results at 25*".
^of
Sat. SoL
Z.0Z4
0.9986
0.9658
0.9268
0.8820
0.8389
0.8370
0.8356
Gms.CdH«0H Gms. HsBOi
per 100 G^. per xoo Gms.
Solvent. Sat. SoL
O
' 8.9
32
SI
70.2
91
93
3
6
99.8
4.11
390
3.58
3.48
3-22
S.06
570
9.Z8
dmoi
Sat. SoL
z.oz8
0.987
0.952
0.908
0.862
0.853
0.842
0.838
0.838
Gms-CtEUOH Gms. per xoo Gms. Sat. SoL
per 100 Gms. * „ ^ _ • — ^ ., ^>^ *
Solvent. HiBO^ CiHiOH.
O
20
40
60
80
8S
90
9S
zoo
S-42
5.20
5.10
S
S05
5.30
6.20
8
ZZ.20
o
Z8.96
37.96
57
75.96
80.50
84.4
87.4
88.8
Solubility of Boric Acn> in Aqueous Solutions of Lactic Acid,
Oxalic Acid, d and i Tartaric Acids at 25*".
In Aq. Lactic Acid.
(Mueller and Abegg, X906.)
In Aq. Oxalic Acid. In Aq. d and i Tartaric Acid.
(Hen, 19x0.) (Herz, x9xx.)
1.0252
1.0722
I.I40S
1.2033
Solvent.
MoL%
CiHdOl.
2.32Z
6.8z9
18.77
36.33
Sat. Sol.
1.0444
Z.0986
z . Z635
1.2254
Gms. HaBOb Gms. per xoooc
per xoo cc. Sat. Sol.
Sat. SoL
Solid Phase.
6.64
9.98
II. S3
Z2.90
HsCaOi. HsBOk.
2.26 6.Z7 HtBOt
6.70
7.44
3.45
0.97
5.36
12.39
ZZ.27
ZO.84
+H,QO«
H,QO«
«i
10.77 o.ss
ZO.63 o
M
Gms. per xoo cc. Sat. SoL
CiBbOk.
HiBQi.
o 5. 59
zz.25iAad 6.20
22.5 " 6.63
45 " 7.48
9.45 « Add 6.ZZ
Z8.90 " 6.48
37 " 7.23
BORIC ACID
156
Solubility of Boric Acid in:
Pure Glycerol (Sp.Gr. -1.260 Aq. Solutions of Glycerol
at 15.5**)- ■ at 25^
iHooper — Pharm. J. Thms. [3] xj* 958. 'Sa) (Hen and Knoch — Z. anorg. Chan. 45, 968, '05.)
<
Sms. Ba0».-
3HK)pcr
100 cc
Glycerine
Gms. B(OH)a per 100
Cms.
Glycerine. Solution.
Wt.%
Glycenne !
in Solvent.
MOUmob
B(OH), per
xoo cc. Sol.
Sp. Gr.
Gms. B(OH)t
per 100
cc. Solution.
Gms.So^
luticn.
0
20
IS 87
13 17
0
90.1
1. 017
SS9
SSo
10
24
19.04
16.00
7IS
90.1
1.038
SS9
5-3^
90
28
22.22
18.21
20
•44
90.6
1.063
5.62
5-28
30
33
26.19
20.75
31
55
92.9
1. 090
S-76
S-29
40
38
30.16
23 17
40
9S
. 97 0
1. 113
6.02
S-4I
so
44
3492
2S-9S
48
7
103.0
^•^33
6.39
S-64
60
SO
39-68
28.41
69
2
140. 2
1.187
8.69
7 32
70
S6
44.65
30.72
ZOO.
0
3903
Z.272
24.20
19. 02
80
61
48.41
32 61
90
67
S3 18
34 70
100
72
S7I4
36.36
In Aqueous Solutions of Glycerol
AT 25**.
(Mueller and Abegg, 1906.)
Aqueous Solutions of Dulcitb
AT 25**.
(Mueller and Abegg, 1906.)
Solvent.
I.IS74
I . 2370
1-2531
Mol. %
OHA.
24.64
46.7s
67.71
9058
aHA.
60
dmm of
Sat. Sol.
Gms. HsBOk
per 100 cc.
Sat. Sol.
Solvent.
"V aH.(OH)«.
0.9995 0.065
I. 0018 0.130
1.0060 0.260
Sat. Sol.
1.0686
I. 0212
1.0260
Gms. HsBQi
per 100 cc.
Sat. Sol.
S-50
S.63
S.81
I. 1707 7.49
1.2260 13.22
90 1.2526 18.3s
96.6 I. 2710 23.44
100 gms. glycerol {du = 1.256) dissolve 11 gms. HtBOt at i5®-i6*'.
(Ossendowski, 1907.)
100 gms. dichloret hylene dissolve 0.006 gm. H3BO1 at 1 5**. (Wester and Bnmis, 1914.)
100 gms. trichlorethyiene dissolve 0.016 gm. HjBOj at 15**. " "
100 cc. anhydrous hydrazine dissolve 55 gms. HiBOi at room temp.
(Welsh and BroderMU, 19x5.)
Solubility of Boric Acid in Aqueous Solutions op Mannite at 25*
AND Vice Versa.
(Ageno and Valla, 191 3, 1913.)
,. , -.. Gms. per xoo cc. Sat. Sol
Grams per 100 cc. Sat. Sol.
H«BOi.
aHuGi.
oouu rnasc
SSO
0
HiBOi
S-90
1.82
6.29
S-46
6.44
7.28
6.64
9. II
6.83
10.93
7.08
12.7s
7.27
14. S7
7.71
18.99
h«bo».
OHmOi.
8.70
2S.6S
9-43
32.43
7.71
27.97
S.7S
2S.6S
4.92
24.65
3 46
23 03
2.87
22.98
1.64
20.80
0
19.58
Solid Phaw.
HsBOs
+QHmO,
CJImO,
<(
«
tc
it
(t
u
ti
Additional determinations at 30'' also given.
Determinations at 25^, differing somewhat from the above, are given by Mueller
and Ab^g (1906). i *
Data for the system boric acid, phenol and water are given by Timmermans
(1907).
157
BORIC ACm
Distribution op Boric Acid between Water and Amyl Alcohol
AT 25**.
(FoK — Z. anorg. Chem. d& 130, '03.)
Millimols B(OH)a in Cms. B(OH)s in xoo cc. MiUimols B(OH)s in Cms. B(OH)i in xoo cc
Aq.
Layer.
265.8
196.5
159.6
126.0
Alcoholic
Layer.
76.6
59 5
47 5
371
Aq.
Layer.
1.648
1. 219
0990
0.781
Alcoholic
Layer.
0.47s
0369
0.294
0.230
Aq.
Layer.
87.9
75-2
64.6
Alcoholic
Layer.
33 a
22.7
19.76
Aq.
Layer.
0545
0.466
0.400
Alcoholic
Layer.
0.206
O.I4I
0.123
Results at I5^ (Maeller and Abegg, 1906.)
MiUimols B(0H). per Liter. Gms. B(OH). per 100 cc. Millimob B(0H). per Gma. B(0H). per 100
Aq. Layer.
894
607.2
589-3
Alcohol
Layer.
264
176.4
177-4
Aq. Layer.
S-44
376
3.65
Alcohol
Layer
1.64
1.09
1. 10
Liter.
Aq. Layer.
427.4
372
289.1
Alcohol
Layer.
127.6
1 10
84.9
cc.
Aq. Layer.
2.65
2.31
1.79
■ ■ ^
Alcohol
Layer.
0.79
0.68
0.53
Data agreeing with those of Fox at 25** are atto given by Muefler and Abegg,
1906. One determination at 35^ gave 0.907 gm. B(OH)i per 100 cc. aq. layer and
0.274 S^i* PCi* i^x) cc. alcohol layer.
Distribution of Boric Acid between Aqueous Sodium Chloride
Solutions and Amyl Alcohol at .25**.
(Mueller aad Abegg, 1906 )
Gms. per
100 cc.:
Gms. per
100 cc:
Aq. Layer.
Alcohol Layer.
HiO. H«BQi.
dm^ of
Alcohol
Layer.
Aq. Layer.
Alcohol^ Layer.
HiO. HsBOb.
d^ci
NaCI. HaBOi.
Naa.
HiBOi.
Alcohol
Layer.
0 5.46
7 3Q
1-65
0.8296
16.64
S13
4. 71
1.79
0.8247
553 5-37
6.40
i.6s
0.8277
17.90
5.02
4.31
1.79
0.8241
8.72 5.27
S-90
1.67
0.8268
20.36
502
4.19
1.87
0.8240
10.91 5.23
5.46
1.69
0.8259
23 52
4.97
3-59
1.96
0.8233
13.84 5.16
5.15
1.77
0.8254
25 03
4. 95
3- 20
1.99
0.8229
Distribution of Boric Acid between Water and Mixtures of Amyl
Alcohol and Carbon Disulfide at 25**.
(Herz and Kurzer, 1910.)
50V0I. %C6HuOH+50
Vol. % CS,.
Gms. HaBOi per 100 cc.
75V0I. %C^HnOH+25
Vol. % CS,.
Gms. HtBOi per 100 cc.
25V0I. %C,HhOH+95
Vol. % CS,.
Gms. HsBOi per 100 cc.
Aqueous
Layer.
0-387
0-743
1. 143
1.590
OHiiOH+CSi.
Layer.
0.09s
O.I7I
0.266
0.365
Aqueous
Layer.
0.469
0.839
1.207
1. 791
aHuOH+CSf.
Layer.
0.095
O.161
0.226
0.344
Aqueous
Layer.
0.433
0.910
1-343
1.940
OHuOH+CSt.'
Layer.
0.053
0.108
0.164
0.238
BORIC ANHYDRIDE B,0,.
Fusion-point data (solubilities, see footnote, p. i) are given for mixtures of
BA+CaO and B,0,-hSrO by Guertler (1904).
BORIC ACID (Tetra) H,B4a.
100 grams water dissolve 2.69 grams HsBiO; at 15*, Sp. Gr. — 1.015.
(Gerlach, 1889.)
BORON TRI-FLUORIDE BF,.
I cc. H,0 absorbs 1.057 cc. BF, at o® and 762 mm.; i cc. cone. H,S04 (Sp. Gr.
1.85) atxBorbs 50 cc. BF,.
B&AS8IDIC ACm 158
B&ASSmiC ACm aHnCHiCHCuHnCOOH.
Solubility data determined by the freezing-point method are given by Mas-
carelli and Sanna (191 5), for mixtures of brassidic and erudc acids and brassidic
and isoerudc acids.
BBOBftAL HYDRATE CBr,.CH(OH)i
The distribution coefficient of bromai 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.
(WinUer— Chem. Ztg. a3» 687, '99; Roonboom — Rec. trav. diim. 3, 99, 59, 73, 84t '84;
J. Ch«m. Soc. IS 477t '63; at i^, Diet» — • Pharm. Ztg. 43, ago. *o8J
unms i»omv
De per xoi
3 ^laniB.
**Ab8orptioa
Coeffident." ♦
"Solttbaity."
%•.
''
Water.
Solution.
(W.)
(R. D. a: D.)
(W.)
(R. D. 8c DO
a.
ff-
0
4.17
4.23
3-98
4 05
60.5
431
5
3 92
3-7
3-77
3 57
45-8
324
10
3 74
3-4
3.61
3 29
35-1
24.8
IS
3 65
3-25
3 52
315
27.0
19.0
30
3 58
3 20
3 46
310
21.3
14.8
25
348
317
3 36
3 07
17 0
II. 7
30
3-44
313
3-32
3 03
13-8
9.4
40 .
3-45
■ • •
3 33
• • •
9.4
6.3
so
3-52
• • ■
3 40
• . •
6.5
4.0
60
...
• • •
• • •
• * •
4.9
2.8
80
...
• • •
• • •
...
30
I.I
* For definition of "Absorption Coefficient " a and "Solubility ' «, see Acetylene, p. z6.
One liter sat. solution of bromine in water contains 0.21 mol. Bri » 33.56
gms. Br at 25**. (Bny and Connolly, 19x0.)
The coefficient of solubility of bromine in water at 15®, determined by an
aspiration method, is given as 33 by Jones (191 1). 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 B&oiaNE in Aqueous Solutions of Mercuric Bromide
AT 25** AND Vice Versa.
(Herz and Paul, 1914.)-
Gms. per xoo oc. Sat. Sol.
HgBr^
O
0.202
0.285
0.462
Br.
3 40
353
3-55
356
Sdid
Phase.
Br2
it
Gms. per xoo cc. Sat. Sol.
SoUd
i(
u
HgBn.
Br.
Phase.
0.763
3-57
Bra+HgBrj
0.701
2.88
HgBr,
0.664
1.20
((
159
Solubility op Bromine in Aqueous' Solutions of Potassium Bromide.
(Results at o^ and 25^, Boericke» 1905; at o**, Jones and Hartmann, 1916;
at iS.s** and 26.5**, Worley» 1905.)
GnuMols
KBr per Liter.
Gin8.KBrp«t
Liter.
o'.
i8.s'.
»s*.
afi.S*.
0
0
41.6 (24.2)
35-56
34
34 23
0.005
0.59
41.7 (25-5)
36.1
34-3
35-1
O.OIO
1. 19
42.6 (26.2)
37
35
36
0.020
2.38
44.4 (27.5)
38-56
36s
37-35
0.050
5.95
so. 2 (31.5)
43-8
41
42 -5
O.IOO
11.90
59. 7 (40)
52 23
49-3
SI. 87
0.20
23.80
79-1 (57.1)
69.69
67 -3
68.69
0.50
59 51
138.6 (hi. 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
1-725
205 . 2
402.3 (395 9)
• ■ •
• • •
• • •
1.82
216.6
423.8 (423)
• • •
• • •
• • •
2.17
258.2
511. 7 (511. 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, Brt.ioHsO, 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 Brs.ioHsO. The results for the latter are shown in parentheses in the
above table.
Solubility of Bromine in Aqueous Solutions op Potassium Svir
phatb, Sodium Sulphate, and op Sodium Nitrate at 25^.
(Jakoirkin — Z. physik. Chem. 30^ 38, '96.)
NomafitTof
Salt Solotun.
InK^SOt
Cms. per liter.
IiiNaaS04
Cms. per liter.
K^504.
91.18
45
22
II
59
79
39
569
Br.
25 14
29.44
31.46
32.70
33 '^o
Na^SO«.
63 -55
31-77
15.88
7-94
3-97
Br.
25.07
29.20
31 -33
32.94
33 26
InNaNOk
Gma. per liter.
NaNO^
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*
CMcLauchlan, 1903.)
Salt.
Water
Na^O*
K.S04
lNH,),SO,
KTaNO,
KNO,
Gma.
Salt per
liter.
0.0
63- 55
91.18
70.04
85.09
loi . 19
Normality
of Dis-
solTedBr.
0.424
0.286
0.310
0.971
0-3495
0.362
Cms.
Br. per
liter.
33-95
239
24.8
77.7
28.0
28.95
Salt.
NH4NO,
IJaCl
KG
NH^Cl
Gma.
Salt per
liter.
80.11
58.50
74.60
53.52
CH,C00NH4 77.09
H,S04* 49-03
NamaHty
of Dis-
solved Br.
0.688
0.701
0.718
1.028
4.26
0.366
Gmt.
Br. per
Uter.
55-15
55-90
57.40
82.2
340.5
29.26
* Wildeman.
i6o
Solubility of Brominb in Aqueous S(h.utions of Sodium Bromide at 25^
(Bell and Buckley, 1912.)
Gnuns per Liter Sat. Sol. ^ of Cms, per Liter Sat. Sot
NaBr. " Br. Sot. Sd. J^I^b^^ ' 57 '
92.6 99.2 1. 213 319.7 546
160.5 176.7 1.372 359 641.6
205.8 247.8 1.515 ... 769.2
255-8 343 1-678 408.3 834
duof
Sat. Sol.
1.997
2.137
2.327
2.420
REaPROCAL Solubility of Bromine and Chlorine, Bromine and Hydro-
BROMic Acid and Bromine and Sulfur Dioxide, Determined by Method
OF Lx)WERiNG OF THE Freezing-point (see footnote, p. i).
Results fo
r Bromine
Bromine + Hyd
ro-
Bromine + Sulfur
+ Chlorine.
bromic Acid.
Dioxide.
(Lebeau, i
Kar^tfn
906; see also
I, 1907)
(BQchner and Karsten, igoft-og.)
(van der Goot, 1913.)
f of
Cms. Br per
t* nf
Cms. Br per
Mol. %
fof
Melting.
Gms. Br per
Melting.
100 Gma.
Mixture.
• in
Melting.
xoo Gms.
Mixture
' Br. in
Mixture.
100 Gms.
Mixture.
-102.5
0
-87.3
0
0
-751
0
— 100
6.5
-90
6
2.5
-75-3*
1.73
- 90
31
-95*
II. 2
4.8
-60
4
- 80
48.6
-90
II. 8
S
-40
12.5
- 70
60.4
-80
lS-2
6.8
-30
21
- 60
70
-70
22
^i-S
— 20
35-5
- SO
79
-60
317
19
~i8
40.5
- 40
86-. 3
-50
43
30
-16
48
- 30
91. 1
-40
54. s
435
-14
72
— 20
95-2
-30
66.2
60
-13
90
— 10
89
— 20
79. S
76.5
— 10
96.5
- 7-3
100
-12.5
90
• Eatec.
90
- 7.1
100
<l
«
«
M
Solubility Data, Determined
p. i), Are Given
Bromine + Methyl alcohol (Maass and Mdntosh, 19x3.)
+ Ethyl alcohol
4- Ethyl acetate
+ Ethyl bromide
4- Iodine
+ Sulfur
100 grams saturated solution
grams Br at —95**, 39 grams at —
BY THE Freezing-point Method (see footnote,
for the Following Mixtures:
II
i<
«
<i
II
rWroczynski and Guye, i9xa )
(Meerum-Terwogt, 1905; Kruyt and Hddcrmann. 1916.)
(Ru£F and Winterfdd, 1903.)
of bromine in carbon disulfide contain 45.4
1 10.5**, and 36.9 grams at — 1 16*.
(Arctowski, 1895 — 1896.)
Distribution of Bromine between Water and Carbon Tetrachloride
Gm. Bn per
Gm. ecu
Solution.
0.01640
0.01847
0.05433
0.06126
Density
CCli-Bn.
1.6454
1.6470
1.6755
1.6809
AT O".
(Jones and Haitmann, 19x6.)
Gms. Bromine per Liter. Gm. Bnpcr
Gm. ecu.
HiO
Layer.
1.28
1.44
4.12
4. 59
ecu
Layer.
26.99
30.45
91.12
103.07
Solution.
0.07261
0.08162
0.08661
o . 1646
Density
CCU-Bn.
1.6896
1.6972
I. 7012
I . 7667
Gms. Bromine per Liter.
HfO
Layer.
5.35
6.03
6.30
11.22
ecu
Layer.
122.82
138.66
184.41
291.10
I6l
DiSTSIBUnON OF BrOMINB at 25** BBTWBBN WaTBR AND:
(Calculated from results of Jakowkin, 1895 « Those in paxentheses from Herz and Kurzer, xgzo.)
Carbon Disulfide.
Bromoform.
Carbon Tetrachloride.
Gms. Br
. per Liter of:
Gms. Br.
per liter of:
Gms. Br
. per Liter of:
Aq. Layer.
CS| Layer. '
Aq. Layer.
CHfirs Layw.
Aq. Layer.
CCI4 Layer.'
OS
I
2
3
36 (35)
80 (75)
163 (155)
240 (230)
o-S
I
3
3
33
66
136
206
O.S
I
2
3
IS (13)
28 (23)
60 (45)
90 (70)
4
5
6
7
330 (310)
420 (39S)
SIS (480)
620 (565)
4
5
6
• . •
276
346
41S
. . •
4
S
6
8
10
12
14
123 (9S)
156 (122)
190 (150)
260 (220)
340 (300)
430 (400)
S20 (550?)
Lewis and Storch (1917) point jout that Jakowkin (1896) failed to take into
consideration, the hydrolysis of the bromine in the aqueous phase in the veiy
dilute solutions. Tney used o.ooi n HCl 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. HsO, divided by the
mol. fraction of Br in the CCI4, is 0.370^ at 25 . These authors also give a series
of determinations of the distribution of bromine between o.i n HBr and CCI4
at 25^
Distribution of Brominb between Water and Mixtures of Carbon
Disulfide and Carbon Tetrachloride at 25^.
(Hers and Kurzer, 19x0.)
25 Vol. -
%CS, + 75Vol.
. 50 Vol. '
% CS,+5o Vol.
75 Vol.
% CS,+25 Vol.
%ccu.
% ecu.
t
^ CCI4.
Gms. Bromine per Liter.
Gms. Bromine per Liter.
Gms. Bromine per Liter.
Aq. Layer
. CSi+CCU Layer.
Aq. Layer.
CSs+CCU Layer.
Aq. Layer
. CSs+CCU Uyer.
0.79
28.4
0.63
28.7
0.71
46
I. S3
S8.4
1. 19
S4.S
1.34
87.2
2.32
86.6
1.76
81. 1
3.98
213.8
2.98
III. 3
2.4S
no. 9
5.06
330.5
3.66
137.8
2.95
132.9
6.82
444.2
5.26
205.1
6.47
343.8
7.9s
324.9
7-97
447.7
9.66
432.2
Distribution of Bromine at 25^ (Herz and Rathmann, 191 3) between;
^ater and Tetn
Grams Bromine
ichlorethane.
( per Liter.
CtHiCli Layer.
6.47
18.20
29.46
41.65
74.57
Water and Pentachlorethane
Gms. Bromine per Liter.
Aq. Layer.
0.216
0.592
0.944
1.348
2.444
Aq. Layer.
0.402
0.670
0.864
1.300
2.408
CaH.Cli Layer.
10.70
18.29
23.49
3S.46
67.44
X62
Data for the Distribution of Bromine between Aqueous Salt Solutions
AND Organic Solvents are Given by the Following Investigators:
Immttdble S<dvents.
Aqueous CdBrs+CCU
Aqueous CdBrs.2KBr+CCU
Aqueous HBr+CCU
Aqueous HgBrs+CCU
Aqueous HgBik.2KBr+CCU
Aqueous KBr+CCU
Aqueous KBr+CSt
f.
25
25
25
25
25
o
Attthority.
(Van Name and Brown, 1917.)
«
M
(Lewis and Stoich, 1917.)
(Hen and Paul, 19x4; Van Name and Brown, 19x7.)
(Van Name and Brown, 191 7.)
(Jones and Hartmann, 19x6.)
32.6 (Roloff. 1894.)
BBOMOrOBM CHBr,.
100 cc. H|0 dissolve 0.125 gm. CHBri at i5**-20®..
(Squire and OJnes, 1905.)
Solubility (Freezing-point lowering data, see footnote, p. i) for
Mixtures of:
Bromoform and Liquid Carbon Dioxide.
(BOchner, 1905-06.)
Bromoform and Toluene.
(Baud, 19x2.)
Gms. CUBa per
; GmA.CHBnper
«
f.
100 Gnu.
CHiBr+COi.
tf o( Fnedng.
^ - 100 Gms.
CHBn+C6Hft.CHs.
Solid Phue.
-31
0
+ 7.7
100
CUBr«
-32
3-7
-II.4
86.6
u
-30
4 9
— 22.2
75.6
€t
-16
13s
-30-9
69.8
tt
- 8
24
-48.5
60,3
l€
- 5
35'
.2-67.7 quad.pt.
- 3-S
92.1
BBUCINE CuH»(OCH,),NtOs.4H|0.
Solubility of Brucine in Several Solvssts.
Solvent. f. ,^^™SJ!i3: Authority.
18-22 0.056-0.125 (MQl]er,'x903;Squ!RandCaines,i9os;Za]ai,x9Xo^
20 12 (ScfaoltE, 1912.)
18-2 2 I . z i-i . 86 (MQller, X903 ; Schaefier, X9X3.)
0.08
1.96
II. 6
2 5
Water
Aniline
Benzene
Carbon Tetrachloride 18-22
« tt
M
f<
20
Chloroform 25
Trichlor Ethylene 15
Ether 18-22
Ethyl Acetate 18-22
Ethyl Alcohol 25
DieUiylamine 20
Methvl Alcohol 25
Petroleum Ether
Glycerol
Pyridine
0.75
4.26
4S-2
1.6
55.6
(Scfainddmeiaer, 1901; God, 19x3.)
(Schaefer, 19x3 .)
(Wester and Bruins, 19x40
(MOUer, X903.)
M
(Schaefer, 19x3.)
(Scholtx, 19x2.)
(Scliaefer, 19x3.)
18-22 0.055-0.088 (Mailer, 1903; Zalai, x9xo.)
18-22 2 . 2 (Mailer, X903-)
20 28 (ScholtE, 19x2.)
20-25 21.9 (Dehn, X9X7.)
20-25 31.6 "
20 I (Scholta, 19x2.)
Ac|. 50% Pyridine
Piperidene
Results for the solubility of brucine and brucine sulfate in mixtures of alcohol^
:hloroform and benzene are given by Schaefer (1913).
BBUCINE Per CHLOBATE CtiHio(OCH,)iNsOt.HC104.
100 gms. H]0(+ 2%HC104) dissolve 0.15 gm. of the salt at I8^
(Ho&nann, Roth, Heboid and Metsler, i9xa)
i63
BBUGINI
BBUCINE SULFATE.
lOO cc. methyl alcohol dissolve 0.28 gm. bnidne sulfate at 25^. (Sduefer, 19x3.)
" ethyl " " 1.66 " " *• " (Schaefcr. 1913.)
" chloroform " 0.6 " " " " (Schaefer. 1913.)
BBUCINE i2, /, and « TARTRATE.
Solubility of Each Optical Isomer in Water (Dotiih, 19x2.)
BUTANE
r.
20
25
35
44
50
C4H10.
Gms. per xoo Cms. Water.
tf Tartrate.
• • •
1.008
1.272
1.590
1.854
/Taitiate.
• • •
1.84
324
4.64
6.56
Raoemic Tartrate.
1.38
• •
Vol. C4H10 per
100 vols. H2O
Solubility in Water at f and 760 mm.
10"
IS*.
9d*.
2.77 2.355
2.147 2.065
3 147
DiphenylBUTADIENE.
Freezing-point curves (solubility, see footnote, p. i), are given by Pascal
(191 4) for mixtures of diphenvlbutadiene and each of the following compounds:
diphenyldiacetylene, diphenylhydrazine and cinnamylidene.
BUTYL ACETATE CHt.CQ1.C4Ht.
Solubility op Butyl Acetate and op Butyl Formate in Mixtxtrbs
op Alcohol and Water.
(Daiicioft — Cak. from Pfeiffer — Fhys. Rer. 3« 105, '95-'960
ec Alcohol
io Mixture.
3
6
9
12
IS
18
21
24
27
30
33
cc. H^ added to cause aeparatioB of a
aecond phase in miztures of the given
quantity of alcohol and 3 cc. portions of:
Butyl Formate.
Butyl Acetata.
3-45
2.08
8.83
6.08
14 -75
10.46
21-45
15 -37
29.65
20.42
39 0
25.60
51.8
31 -49
00
37 48
43-75
50.74
59-97
too oc H^ dissolve 0.7 cc. isobutyl acetate at 2 j^.
IsoBUTTL ACETATE, etc.
Solubility in Water. CTtaube, 1884; at 90*, Vaubd, X899O
(BBncRift4
Compound*
22
22
20
20
Iso Butyl Acetate
Iso Butyl Formate
Normal Butyric Aldehyde
Iso Butyric Aldehyde
Grams Com-
pound per 100
Grams HiO*
0.5
I-O
10 -o
BUTTL ALCOHOLS 164
Secondary BUTYL ALCOHOL CHt.CHOH.CHsCH|.
Iso BUTYL ALCOHOL (CHt)tCH.CUsOH.
Solubility of Butyl Alcohols in Water, "Synthetic Method/'
(see Note, p. 16).
M8860
SeoonHary Butyl Alcohol Iso Butyl Alcohol
and Water. and Water.
Gma. Secondtfy Butyl AkxAol per 100 Gmi. Gmi. lao Bptyl Alcohol per 100 Cms.
^o Aqueous Alcoholic Aqueous Alcohdic
Layer. Layer. Layer. Layer.
—20 27 66 ... ...
— 10 28 60 ... ...
o 27.5 56 13 85
10 26.0 57
20 22.5 60 9 84
30 18 63.5
40 16 65.5 7.5 83
60 13 67 7 82
80 IS 63 7 77.5
100 20 5a 8 72
107 crit. temp. 33
Xdo z6 62
130 28 so
133 crit temp. 49
Additional determinations of) the reciprocal solubility of secondary butyl
alcohol and water are given by Dolgolenko (1908). This investigator prepared
three fractions of 98®-98.6®, 98.6*^-99** and 99*^-99.5® boiling jioint 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 COj (BQchner, 19QS-06.)
Normal butyl alcohol + Water (Dreyer, 1913.)
" " " + Liquid COj (BOchner, 1905-06.)
Secondary butyl alcohol + Water (Dreyer, 1913; Timmermaiis, 1907, 1910, 1911.)
" ^" " + " + Hydroquinine (Tinunermaiis, X907.)
Tertiary butyl alcohol + Water. (Dreyer, 1913O
i65 IsoBUTTI ALCOHOL
Distribution op Isobutyl Alcohol bbtwbbn Water and Cotton Sbbd
Oil at 25^ (Wroth and Reid, 19x6.)
Gma. C4H1OH per too cc Ghm. CiHiOH per 100 cc.
Oa Layer. HiO Layer. Ratio. PU Layer. H^ Layer. Ratio
1. 168 2.043 1-74 I -375 2.301 1.67
1.276 2.250 1.76 1*405 2.429 1.72
1.288 2.135 i-^S I-49S 2.450 1.64
The partition coefficient of tertiary butyl alcohol (CHi)iC(OH)CHi, between
olive oil and water is given as 0.176 at ord. temp. (Baum, 1899.)
IsoBUTTLAMINX HTDBOCHLORIDE (CH,),CHCH,NH,.HC1.
100 g:ms. HsO dissolve 238.9 gms. of the salt at 25^ (Peddle and Tomer. 19x3.)
100 gms. CHCli dissolve 11.56 gms. of the salt at 25^ (Peddk and Turner, 1913.)
BUTTLCHLORAL CH,CHC1.CCUCH0.
The distribution coefficient of butylchloral betweem oil and water b given as 1.6.
(Meyer, 1907.)
BUT7LCHL0RALHTDRATE CH,CHCl.CClt.CH(OH)s.
,0
100 gms. H^ dissolve 2.7 gms. butylchloralhydrate at 1^.5*
(Greenish and Smith, 1903.)
2.3 " " at I5*^-2o^
(Squire and Caines, 1903.)
" glycerol " 100 " " at 15^-20*.
(Greoiiah and South, 1903 •)
The partition coefficient of butylchloralhydrate between olive oil and water is
given as 1.589 at ord. temp. (Baum, x899-)
BUTTBIC ACIDS (normal) CH,(CHi),COOH; (iso) (CH,),CH.C(DOH.
SOLUBfLITY OF NORMAL BUTYRIC ACID IN WaTBR, DbTERMINBD BY THB
Freezing-point Method. (Fauom, 1909, X910.)
f of
Gms. Acid per
100 Gms.
Mixture.
f of
Gms. Acid per
xoo Gms.
Mixture.
fof
Gms. Add per xoo
^mgeating.
Congealing.
Congealing.
Gms. Mixture
0
0
- 3-57
67.38
-13-40
87.62 Eutec.
-1. 08
5"
- 5.20
75
— 12.40
90.08
— 2.70
12.7s
- 6.80
80
— 10
95-92
— 2.96
25-32
- 8.61
84
- 8
98.60
-3 07
50.60
-10.25
85.41
- S-40
99-15
-3 14
59-72
-12.54
86.54
— 3-12
100
Higher values for the temperature of congealing of the above mixtures are
given by Ballo (1910). For additional data see also Timmermans (1907) and
Tsalcdotos (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 comfiletely 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, —45 —7
Gms. acid per 100
i gms. mixture 25 30 35 40 50 58.2
Solubility op Isobutyric Acm in Water, Determined by the Freezing-
point Method. (Faucon, 19 Eo.)
The congealing temperatures for mixtures containing up to 60 grams iso-
butyric add ^ 100 gms. coincide with the results given in the above table for
normal butync acid and water. For higher concentrations the following results
were obtained.
t® of congealing —309 —3-35 — 3-6i —12.5 —80
Gms. add per 100
gms. mixture 70.10 82.08 86.44 97 -21 100
BUTYRIC ACID l66
MiSCIBILITT OF ISOBUTYRIC AciD AND WaTBR, DBTBRMINBD BT THB
"Synthetic Method."
(Smixnoff, 1907.)
Gms.'Add per i
[oo Gms.:
f.
Upper Layer.
Lower Layer.
10.05
69.08
17.82
12
67.1
18.3
14
64.9
19. 1
16
62.3
20
18
59-2
21. 1
20
554
22.8
22
49
25.8
22.5
46
27
23
41
29
23.3crit.t.
34.7
Detenninations varying more or less from the above are given by Rothmund
(18^8), Friedlander (1901; and Faucon (1910). The discrepancies s^re shown by
Smirnoff to be due to the effect of variations in purity of the isobutyric acid upon
the position of the curve. Smirnoff fractionate the purest obtainable acid and
determined the miscibility curve for each fraction. The above results were
obtained with fraction 4 of boiling point 154^-155*1 twice refractionated.
An extensive series of determinations are given by Smirnoff of the effect of
various percentag:es of different salts upon the temperature of immiscibility of
aqueous 16.46% isobutyric acid solution.
Distribution of Butyric Acid bbtwsbn Watsr and Benzene at 13^-15*
(Geozfievics, 19x3.)
Gms. Butyric Acid
Uicd.
Gms. Add Found per*
tM.
X50CC.
Benzene Layer.
25 CC
HiO Layer.
2.0044
2.9968
3 . 5028
4.0088
I 7643
2.6965
3 1740
3 6544
0.2401
0.3003
0.3288
0.3544
4 . 5342
4.1521
0.3821
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
CaClt 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. (Crowdl, 19x80
Data for the Following Ternary Systems Containing Normal
Butyric Acid are Given by Timmermans, 1907.
Normal Butyric acid + Water + Azobenzene.
*^ " " + Barium nitrate-
-[- Benzophenone.
4- Camphor.
+ Cane sugar.
4- Mannite.
4- Naphthalene.
4- Potassium sulfate.
4- Sodium chloride.
Freezing-point data are given for mixtures of n butyric acid and formamide by
English and Turner (191 5), and for mixtures of trichlorobutyric acid and dimethyl
pyrone by Kendall (19 14).
<l
II
l<
II
u
II
II
II
(1
If
II
II
II
II
167 CADMIUM BBOMIDS
OADMIUM BROMIDE CdBr,.
Solubility in Water.
(Diets— Ber. 39, oS* '99; Z. anon;. Chem. ao^ 960, '99; Wiss. Abb. p.t. Reicbanstalt 3» 433i '00; tee afao
Eder — iMngier polyt. J. aai« 189. '76; Etard — Ann. chim. phys. [7] a, 536, ^4*)
Gmt. CdBra Mob.CdBr)
Solid Pbaae. t". per 100 Gms. per xoo Solid Pluae.
Solution. Mols. HjO.
CdBr2.4H,0 40 60. 65 10.20 CdBr2.H20
" 4S 60.75 10.24 "
" 60 61. lo 10.39 "
" 80 62.29 1048 "
t«.
Onw-CdBra Mols.CdBrs
per zoo Cms. per 100
Solution. Mols. HsO.
0
18
37 -Q*
48.90
4.04.
6.21
30
38
56.90
61.84
8-73
10.73
35
60.29
10.05 <
u
CdBr,.HaO 100 61.63 10.63
Density of saturated solution at i8^» 1.683.
Solubility of Cadmium Bromide in Alcohol, Ether, Etc.
100 gms. sat. solution of CdBri.4HiO in abs. alcohol contain 20.93 gms. CdBri
at 15**. (Eder.)
100 gms. sat. solution of CdBrs4Hi0 in abs. ether contain 0.4 gm. CdBr^ at 1$°.
(Eder.)
100 gms. absolute acetone dissolve 1.559 gms. CdBrs at 18^. d^ sat. sol. »
0.8073. (Naumann, 1904.)
100 gms. benzonitrile dissolve 0.857 gm. CdBrs at 18^. (Naumann, 19x4.)
100 gms. anhydrous hydrazine dissolve 4O gm. CdBri at room temp.
(Welab and Broderson, 19x5.)
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, X907; Ruff and PUto, X903.)
4- Cadmium Iodide (Nacken, X907.)
-j- Calcium Fluoride (Ruff and Plato, X903.)
+ Cuprous Bromide (Herrmann, x9xx.)
+ Potassium Bromide (Brand, 19x3.)
+ Sodium Bromide "
+ " " + Potassium Bromide "
14
14
44
II
41
14
CADMIUM (Mono)AMMONn7M BROMIDE CdBrs.NHtBr
Solubility in Water.
(Rimbach, 1905; Eder.)
100 Grams Solution contain Gms. Atomic Relation. G.CdBrfJIHiBr
*• 'Cd! bT, nS.. Cd : Br : NH«: "m'So?."*'
1.0 16.33 34.87 2.63 I 3 1 53.82
14.8 17.40 37.15 2. 80 131 58.01
52.2 19.79 42-38 3-21 1 3 I 65.31
110. 1 22.99 49.17 3.72 131 75.98
100 gms. sat. solution of CdBra.NH4Br in abs. alcohol contain 15.8
gms. double salt at i;^ (Eder).
xoo gms. sat. solution of CdBra.NH4Br in abs. ether contain 0.36
g^. double salt at 15^ (Eder).
GAOODmO ACm (CHOtAsO.OH.
100 cc. HsO dissolve about 200 gms. cacodylic acid at 15^. (Squire and (Raines, igosO
XOO cc. 90% alcohol dissolve about 28.5 gms. cacodylic acid at 15^ " "
CADMIUM BEOMIDS
168
OADMIVM (Tetra) AMMONIUM BROMIDE CdBr,.4NH4Br.
Solubility in Watbr,
(Rimbach.)
The double salt is decomposed by water at temperatures below i6^**c
.ON
xoo Gnu. Solution contain Gnu. Atomic Relation in Sol. Atomic Rdation in Solid.
• •
Cd.
Br.
NH4. Cd : Br :
NH«. ' Cd : Br :
NH4.
0.8
14.72
50.46
6.67 ]
[ 4.82
2.82. ]
[ 10.02
8.02
13 o
14. 95
51 48
6.85 ]
c 4-85
2.85 ]
c "57
9-57
440
15.01
53-85
7-35 3
c 5.04
3.04 J
[ 6.84
4-84
76.4
14.6
55-28
7.80 ]
t 532
3 32 3
c 6.63
4 63
"3 5
^S'S
5950
8.45 1
^ 5-38
3-3^ 3
[ 7.40
540
160.0
14.7
62.67
9-43 3
t 5-99
3-99 J
[ 6.03
4 03
CADMIUM (Mono) POTASSIUM BROMIDE CdBr,.KBr.H,0.
Solubility in Water.
(Rimbacfa; see alao Eder.)
0.4
X5.8
50-0
112. 5
XOO Gms. Solution contain Gms.
£dr
Br.
5-42
15-41 33 -o
16.85 35 96 5.86
19.58 41.86 6.85
22.24 48.28 8.14
Atomic Relation in Sol.
'Cd
X
I
I
098
Br
3
3
3
3
I
X
X
I
03
Gm9.CdBr|JCBr
per xoo Gi
Solution.
53 63
58.61
67.87
78.11
CADMIUM TetraPOTASSIXTM BROMIDE is decxnnposed by water at
ordinary temperatures.
CADMIUM (Mono)RUBIDIUM BROMIDE CdBri.RbBr.
0.4
14-5
49.2
107.5
100 Gms.
SoLUBiLrrY IN Water.
(Rimhacb.)
Solution contain Gms. Atomic I
Ulation in Sol.
Br : Rb.^
3 1^01
3 I 01
3 I
3 0.96
Gms. CdBn.RbBr
Cd.
8.37
10.72
15.01
19.65
Br.
17-93
23.02
32.13
41.12
Rb. Cd :
6.43 I
8.30 0.99
II. 51 I
14.06 1.02
Solution.
32-65
41.87
58.54
75-77
CADMIUM (Tetra)RUBIDIUM BROMIDE CdBrs.4RbBr.
Solubility
IN
Water.
(Rimbach.)
f.
xoo Gms. Solution contain Gms.
Atomic kelation
in Sol.
Gms.CdBri.4ltbBr
Cd
Br
Rb. '
'Cd : '
Br :
Rb.
Solution.
0
■5
5 70
24.94
17.97
0.98
6
4.05
47-95
13
•S
6.55
28.74
20.74
0.97
6
4.05
55-17
SI
•5
8.25
35.51
25 -39
0.99
6
4.02
68.82
"4-5
9-50
40.67
29.00
t
1. 00
6
4.0
79.04
169
CADMIUM BBOMXDX
CADMIUM (Mono) 80DIX7M BB6MIDX C(lBr,.NaBr2iH,0.
Solubility in Water, etc., at 15®.
(Eder — Ding, polyt. J. aaz, iS9,'J'j6^
Cms. CdBn JTftBr per xoo Gmi.
oonvm*
Water
Absolute Alcohol
Absolute Ether
Solution.
49.0
31. a
0.53
Solvent.'
96.1
37.0
0.53
SolU
Phaae.
CdBr,.NaBr.3iHaO
It
CADMIUM CHLORATE Cd(C10,)i.2HiO.
S(H.UBiLiTY IN Water.
(MeusBer, 1903 )
Cms. ' Mols.
* * per zoo Gms. per 100 Mols.
Solution. HiO. ^
— 6.5 26.18 3.07 Ice
-130 52.36 9 52
— 20.0 72.10 22.47 Cd(aOi)i.aHiO
72.53 22.87
Gntt. Mob.
^ Cd(C10i)i Cd(C10>)i
* per xoo Gma. per xoo
Solution. Mols. H«0.
Solid Phase.
-15.0
Density of the sat. solution at 18^ » 2.284
± o
18
49
6S
74.95 25.92 Cd(C10^t.2Hi0
76.36 27.98
80.08 34.82
82.95 42.14
CADMIUM CHLORIDE CdCli.2iHi0.
Solubility in Water.
(Dfeti — W. Abh. p. t. Rdchanstalt 3, 433* '00; above xoo^ Etard — Ann. cUm.pliys.[7] a, 536, '944
Mols-CdO.
per 100
Mob.HtO.
G. CdCls perMol8.CdCl3
100 Gms. per xoo
Solntioa. Mols.HaO.
SoUd
Phase.
G.CdCkper
100 Gms.
Solution.
SoUd
Phase.
- 9
o
+10
IS
— 10
o
fi8
30
36
43 58
49 39
S9"
44-35
47-37
52.53
56.91
57 91
7.5
9.6
12.3
14.2
7.8
9.0
10.9
13.8
13 -5 J
CdCl,.4H,0
+ 10 57.47
20 57-35
40 57-51
60 57.71
80 58.41
100 59 52
CdCla.3iH,0 150 64.8
200 73.0
270 77.7
13 -3
13.3
13 -4
13-8
14.4J
CdCl,.I^O
(moDodinic)
Density of saturated solution at i8* « 1.741.
100 gms. abs. ethyl alcohol dissolve 1.52 gms. CdCli at I5*.5.
100 gms. abs. methyl alcohol dissolve 1.71 gms. CdClt at I5*.5. (de Bniyn, x89s.)
100 gms. abs. methyl alcohol dissolve 1.5 gms. CdClt at the crit. temp.
(Centnerszwer, 19 10.)
100 gms. benzonitrile dissolve 0.063 gni. CdCli at I8^ (Naumaan, 19x4.)
GADMIUM GHLOBIDI 170
Reciprocal Solubilities, Dbtbrminsd by the Method op Lowbsing op
THE Freezing-point (see footnotet p. i)» Are Given por the Following
Mixtures:
Cadmium Chloride + Cadmium Iodide (Nacken, 1907 (c); RufF and Plato, 190130
" " -j- Cadmium Fluoride (Ruff and Plato, 1903)
" " + Cadmium Sulfate
" " + Calcium Chloride (Sandonninl, 191 z, X914; McoffB, Z911O
" " -}- Cuprous Chloride (Hemnann, 191 z.)
** ** 4* Lead Chloride (Sandcnmini, 191a, Z9Z4; Hemnann, z9xz.)
+ Magnesium Chloride (Menge, zgzz.)
+ Manganese Chloride (Sandonnmi, Z914; Sandnnnfni and Scarpa, 1911O
+ Mercuric Iodide ^ (Sandonnini, Z9ia.)
+ Potassium Chloride (Brand, z9zi.)
+ Sodium Chloride
-j- " " + Potassium Chloride (Brand, 1911.)
+ Strontium Chloride (Sandonnini, 191 z; Z9Z4.)
+ Thallium Chloride (Korreng, Z9Z4', Sandonnii^ 19Z3.)
+ Tin (ous) Chloride (Herrmann, X9iz; Sandnnnini, X9Z4O
+ Zinc Chloride CBemnann, Z9zz.)
i< II
II II
II II
II II
II II
II II
II II
II II
II II
41 tt
OADMIUlf AMMOHIUlf OHLOBIDI CdCU.NH4a
Solubility in Water.
(Rimbach — Ber. 30^ 9075, Z897.)
%•.
100 Gma.
Sdntion contain Gma.
Gma. (M(3sllH4Cl per zoo GaA
'Cd.
CI.
NH .
Soltttian. Water. '
2.4
14.26
13-44
2.24
29.94 42.74
16.0
iS-Sa
IS 07
2.56
33-45 50.26
41.2
18.61
17.46
2.89
38.96 63.83
63.8
20. 92
19-73
3-34
43 99 7854
105.9
24.70
23-52
401
52.23 109.33
OADMIUM (Tetia) AMMOHIUM OHLOBIDI CdCl,.4NH4a.
In Contact with Water.
The salt is decomposed in aqueous solution.
(Rimbach.)
^ • zoo Gms. Solution contain Gma. Atomic Relation In Solutloo.
• .
Cd.
a.
N114.
Cd
: a :
NH«:
3-9
5-75
18.17
7-37
9.96
7.96
16. 1
6.96
20.26
7-97
9.20
7-13
40.2
9.91
23-84
8.92
7.61
5.61
58-5
12.50
26-53
9-35
6.71
4.66
Z12.9
16.66
31-79
10.78
6.02
4 02
"3-9
16.51
32.71
11.30
6.26
4.26
Solubility of Mixtures of Cadmium Tbtra Ammonium Chloridb
AND Cadmium Ammonium Chloride in Water.
(Rimbach — Ber. 3S» 1300, 'oa.)
t».
zoo Gma.
Solution contain Gms.
Atomic Relation.
Solid]
Mol.per
CdOiL
NH«a.
E^haae.
oent of:
Cd.
a.
NH«.
Cd
: Q :
NH«.
CdOa.
4NH^
I.Z
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 0
53 0
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 GHLOBIDX
SOLUBIUTT OF MiXTURBS OP CaDMIUM TbTRA AmMONIUM CHLORIDI
AND Ammonium Chloridb in Watbr.
(RimbftchO
100 Gms. Solntko
Atomic
SoHd Phase.
»•.
contain Gnu.
Relation.
Mol.
per cent of:
Cd. a. NH.
(T
: a :
NH«.
'NH«a.
CdOa-HNHA
I.O
2. 83 17. II 7.8a
I
19.21
17.28
59 0
41 0
13 a
2.76 18.84 8.71
I
21.62
19.62
74 0
26.0
40.1
3.16 23.56 10.49
I
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
OADMIUM BABIUM OHLOBIDS a(Cda,)BaCl,.5H,0.
Solubility in Water.
(Rimbach — Ber. 30, 3083, '97.)
zoo Cms. Solution
Gms. a(CdC3a)£aCb
f.
contain Gim.
per zoo
Gms.
Cd.
a.
" Bk.
Solution.
Water.
22.6
17.71
16.89
II. 0
45.60
83.82
41.3
19.22
18.15
11.77
49.14
96.62
53-9
19.85
18.7s
12.41
51.04
104.25
62.2
20.59
19.66
12.83
S3 08
"3 13
69 S
21.20
20.18
13 09
5447
119.64
107.2
24.25
23-23
14.90
62.38
165.85
OADMIUM BARIUM OHLOBIDS CdCl,.BaCl,.4H.O.
Solubility in Watbr.
(Rimbach.)
zoo Gms. Solution
Gms. CdOsRaCIs
%•.
contain Gms.
per 100
Gms.
Cd.
a.
Ba.
Solution.
Wattf.
22.5
11.98
IS 19
14.71
41.88
72.06
32 -9
12.40
16.18
16.09
44.67
80.73
41.4
^3 OS
16.95
16.81
46.81
88.01
53-4
13.96
18.21
18.13
SO. 30
IOI.2I
62.0
14-73
18.81
18.74
52.28
109.56
97.8
I7S7
22.48
22.00
62.05
163 .50
108.3
18.53
^3S^
22.79
64.83
184-33
109.2
18.67
23.69
29 -95
6S-3I
188.27
OADMIUM MAOBBtlUM OHLOBIDS 2(CdCl,)MgCl,.i2HA
Solubility in Water.
(Rimbach.)
xoo Gms. Sohitiao
Gms. a(Cd<
:is).MgCii
%•.
contain Gms.
per 100
Gms.
Cd.
a.
Mg.
Solutian.
Water.
2.4
22.14
21.06
2.41
4S-6i
83.86
ao.8
24-30
22.80
^'5S
49.69
98.77
4SS
26.24
24 ss
2.72
S3 SI
115.10
67.2
28.45
26.71
2.98
S8-I4
138.90
21.8
31.84
30.20
3-44
65.48
189.69
CADMIUM CBLOBIDX
172
CADMIUM (Mono)BUBIDIUM CHLOBIDI CdCli.Rba.
Solubility of Cadmium Monorubidium Chloride in Watbr.
(Rimbach, 190a.)
100 Gms. Solution contain Gms.
Cms. CdGt.RbCl per 100 Gmi.
• •
' Cd.
a.
Rb. '
Solution.
Water.
X.2
4.80
4-53
3 63
12.97
14.90
I4S
6.20
5-88
4. 75
16.80
30.19
41-4
9-34
8.86
714
25 31
33 89
57-6
11.40
10.78
8.63
3083
4458
103.9
17.14
16.37
13 -39
46.62
87.36
CADMIUM (Tetra)BUBIDIUM CHLOBIDI CdC]t4Rba
In Contact with Watbr.
The double salt decomposes to CdClj.RbCl and RbQ.
%•.
100 Gms. Solutioo contain Gnu.
Atomic Relatioa.
Moi. per cent of:
Cd.
a.
Rb.
Cd : Q : Rb.
CdQi. CdCls.
RbQ. 4RbCf.
0.7
8.8
13.8
0.65
1.07
1-32
6.52
7-37
7.86
14-73
16.13
16.93
I 31.88 29.88
I 21.89 19.89
I 18.88 16.83
30 70 ^
24 76
16 84
42.4
3-21
"•35
22. 45
I II. 21 9.21
14 86
59 0
108.4
4.61
8.94
13-41
18-57
25-31
31-15
I 9.23 7.23
I 6.57 4-59
33 67
• • • •
Solubility op Mixtures op CdCl,.4RbCl and RbCl in Water.
(Rimbach.)
Solid Phaie,
t*.
0.4
14.8
17.9
100 Gms. Solution contain Gms.
Cd.
a.
12.86
13.62
14.0
Rb.
30 -97
32.81
33-71
Mol. per cent of:
Atomic Relatioa.
r5. cdaa.4Rba rScl
I 55 45
Cd
a
I
I
I
I
I
67
80
33
20
The Effect of the Presence op HCl, Cad and of LiCl upon
amoN OF Cadmium Tbtrarubidium Chloride by Water at
Decomfo-
16*.
100 Gms. Solutioo contain Gms.
Total a.
3^-44
28.45
12.09
14.98
12.70
10.85
9.08
26.49
ao.37
CL
0.84
0.80
3-«4
Ck.
7 56
S-77
3 78
1.84
li.
4.87
3-33
HQ.
36.61
28.44
9. II
CaQa.
20.91
15.96
14 -47
5.10
liO.
29.40
20 'II
Cd.
0.4Z
0.3s
0.69
073
0.77
1. 00
1 .24
0.56
052
Rb.
1-39
1.38
6.74
2.80
4.87
8.51
12.14
3-871
7.84
Mds. per ico Mois. HgO. Molecular Ratio.
CdCls. RbOl BCT CdQi : RbO:
0109 0.483 29.76 I 4.43
0.082 0.422 20.3s ' 5-'5
0.139 1.772 5.60 X 12.75
CaQs.
0.159 0.799 4-59 » S-04
0-163 1.353 3-41 I 8.31
0.2II 2.365 2.24 Z 11.22
0.262 3.385 1.09 z za.92
ua.
0139 1. 271 19.40 I 9.13
0.122 2.433 12.54 I 19.88
See Note on next page.
ITS CASUQIK OBbOBIDB
OAOMIUM (Mooo) VOTASSIUM OHI.OmiDS CdCU.Ka.H,0.
SOLUBIUTT IN WaTSIU
Cd.
a.
iL
a. 6
9 53
9 03
3 31
15 9
11.63
10.98
3 99
41 5
15-47
14-73
5-45
6o.6
17.68
16.80
6.20
105.1
aa.46
ai-34
7.87
p«r ICO l«m».
"87 •7 99
16.60 36.14
3566 SS34
40. 67 68.55
51 67 Z06.9X
OADMIUK (Tetra) FOTASSIITK OHLOBIDS CdCU.4Ka.
In Contact with Water,
(RimbttchO
The double salt is decomposed when dissolved in water at ordinary
too GniBs Sohitioa contalB Gmi.
t\ . .
Cd. a. K,
4 3 64 9-^ 8.31
93.6 5.66 14.03 11.51 %
50.1 9.10 18.09 13.60
108.9 11-94 13.11 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 8alt» were
plotted on cross-section paper, and the points at which the decom-
position was prevented, were determined by interpolation. These
values which snow the minimum amount of the added chlorides which
must be present to insure the crystallization of the pure double salt are
^own in the following table.
Added
Oilnride.
HCl
LiCl
CaCl,
KCl
Mob.
CdOi.
0.074
0.344
0.544
X.034
per xoo Mblfl. HsO.~
X^P, Addwil
*•"• Chloride.
0-196 19.80
1376 930
1.176 3.80
6.514* 3-37^
Denilty of
Sdutiooa.
X.I403
X.I380
1-2333
Z.II4
Moll.
per Liter of Solution.
CdOi.
0033
0.166
0.370
0.507
Ypi Added ^
'^^»- Chloride.
0x31 8.818
0.663 4.483
1.080 Z.887
3 . 195* z . 167
•ToUL
CADBOUM CHLOBIDI
174
S(x.uBiLiTY OP Cadmium Chloride in Aqueous Solutions of Potassium
Chloride at Several Temperatures and Vice Versa. (Sudhaus, 1914)
Gmt. per loo gms. H«0.
CdCls. KCT
Results at 19.3^
III. 3
59 59
♦26.98
II .61
1.44
0.0
0.0
6.7
11.09
30.04
34.76
33-94
Results at 29.7*
129.65
97.62
68.23
47.12
*32.67
24.^6
iS-99
15-47
2.42
0.0
Di.i.i
0.0
0.70
7.08
9.89
13.06
16.10
25.97
33.58
37.66
37.21
Solid PhMe.
CdCl,.2iH,0
Di-i.i
Diu+KCl
KCl
CdCli.2}HiO
"+D1.M
tt
it
u
" +Dm
Dm+KC1
KCl
Gmt. per lop gms. H^.
ddcC ' KCiT
Results at 40.1 ^
133-85
92.15
SI -90
*37-9i
24-45
18.97
19.92
2.98
0.0
0.0
2.70
11.50
15.21
21.73
35-51
37-63
40.45
40.36
Results at 54.5.
133-9
102.15
♦44.01
26.13
4.20
0.0
0.0
2.32
18.39
43-78
45 52
43-00
Solid Phaae.
CdCl,.H,0
" + Di.M
Di.i-i
tt
tt
tt
D1.4+KC1
KCl
CdCl,.IW)
" +Dm.i
Di-i-i
" +D1.4
D1.4+KCI
KCl
CdCl,.KCl.HiO, D1.4 - CdCIt^KCl.
* Show* the solubility of the double salt in water.
Solubility of the Double Salt. CdCli.4KCl in Water. (Sudhaua, 19x4^
f.
19-3
23.6
29.7
40.1
50.2
54.5
Cms. CdGs.4KG per
100 gms. xUO.
41.65
45-35
49-05
57.55
68.89
Mol. Ratio in Solution.
iCdCl»: 6.37 KCl
:5-85
= 5-34
:4.6o
:4-30
: 4.12
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
69.91
Solubility op Cadmium Chloride in Aqueous Solutions of Sodium Chloride
AT Several Temperatures and Vice Versa. (Sudhaus, 19x4.)
Gms. per loo gma. H«0.
CdClt. NaCl. '
Results at I9.3^
Solid Phase.
Gms. per loo Rms. HiO.
Solid Phaae.
III. 30
116.64
85-15
♦40.01
5.96
0.0
0.0
7.52
12.19
25.67
36.76
35.84
CdCl,.2§H,0
((
" +Naa
NaCl
Results at 29.7^
CdCb. Naa.
Results at 29.7* (con.).
♦43.74 27.46 D1.2.S
9.43 37-54 " +Naa
Results at 40.1^.
137.03 15-14 CdCli.HiO+DM.!
♦48.17 29.50 Dm.s
13.31 38.16 " +NaCl
Results at 54.5*.
19.10 CdCl,.H20+Di.i.«
32.97
39.07
36.82
132.67 9.63 CdCls.2|HsO+Di.2.8 140.42
123.54 10.10 D1.1.S *52.76
106.16 12.92 " 22.53
91.10 15.41 " 0.0
Di.t.i - CdClt.2NaC1.3H,0.
* Shows the solubility of the double salt in water.
CADBOUM GINNABIATE8 (C<HtCH :CH.COO)sCd.
100 gms. water dissolve 0.070 gm. cadmium cinnamate at 26^.
100 " " " 0,56 " cadmium isocinnamate at 20".
100 " " ." 0.10 " cadmium allocinnaiDate at 20*
D1.S.8
" +NaCl
NaCl
(de Jong, 1909.)
(Michael, 1903.)
ITS
GADMnni CTllllDB
GABMIUII CTllllDB Cd(CN)>.
loo gms. HdO dissolve 1.7 gms. Cd(CN)t at 15*.
GABMIUII FLUOSIIII CdF«.
tttt^
100 oc of sat. solutioii in water oontsin 4^ gms^ CsFt at 25*.
100 oc of sat. solodoa in 1.08 n. HF contain 5*62 gms^ CaFt at 25*. (jMiEcr, 19014
iFreezing-pobit lowering data (solubility, see footnote, jk i) are given for nux«
tmes of camnium fluoride and cadmium iodide by Ruff and Plato (1903), and
for miztoies of cadmium fluoride and sodium fluoride by Puscbin and Baakov»
(1913).
Cd(OH)i.
SOLUBIUTT IN WaTBK.
I liter of axnieoos solutkn contains aoo26 gm. Cd(OH)t at 25*.
(BodBste.tSM
SOLUBIUTT IN AqUBOUS AMMONIUM HtDROXIDB SOLUTIONS.
«
Results at 25^
Results at 16-21*.
(BoBKkdl, 19040
(Eufer, i9oaO
Noniafily ol
I Gm.Cd(OH)i
*•
Nonufityof Gi
B».Cd(0H)t
NHs.
per liter.
w .
NHi.
per liter.
OS
0.274
16-17
0.47
0.44
I.O
0.707
<C
0.87
X.I7
1.8
1.516
21
0.26
0.09
4.6
S.609
cc
o^sx
0.32
AD]
linJM lODnXB Cdls.
SOLUBIUTT IN WaTBR.
(DietB, 1900: see abo Kremen, 1858; Eder, t8;6; Etud, 1894.)
4»
Gmft-Oflaper
xoo Gms. Mob. Cdli
*•
Gm. Cdb per 100 Gms.
Mob-Cdb
W m
' Solution.
Water.' mS. BM).
m •
Soltttioa. Water.
per 100
Mob-HiO.
0
44-4
79.8 3.9
30
47-3 89.7
4-43
ID
454
83.2 4.1
40
48.4 93-8
4.6
15
45. 8
84.5 4.17
SO
49-35 97.4
4.8
18
46.02
85.2 4.2
75
52.65 III. a
S-4
20
46.3
86.2 4.26
100
56.08 127.6
6.3
25
46.8
87.9 4.34
Density of saturated solution at 18* ~ i*590.
Solubility of Cadmium Iodidb in Organic Solvbnts.
Gms. Cdh per xoo Gms.
"Solvent t*.
Absolute Alcohol 1 5
Ethyl Alcohol 20
Methyl Alcohol 20
Propyl Alcohol 20
Absolute Acetone 18
Benzonitrile 18
Ethyl Acetate 18
Ethyl Ether 12**
Anhy. Hydra2dne 15-20
Benzene 16.0
35 -o
?*i-.994.
Solution. Solvent.
50.5 102
42.6 74.27
59.0 143 -7
28.9 40.67
20 25*
Z.63
i.84t
0.143
84 1
0.047
0.094
t *•- .9143.
Observer.
(Eder.)
(Timofeiew, 1891.)
(Tlmoteiew, 1891.)
(Timofeiew, x89c0
(Naumann, 1904^
(Naumann, x9X4<)
(Naumann, 1910.)
(Tyrer. 19x1.)
(Welsh and Brodenoo, t9t5^
(Linebaifer, 1895.)
X ptt xoooc*
CADMIUM lODIDI
176
Solubility op Cadmium Iodide in Methyl Alcohol, Ethyl Alcohol, Propyl
Alcohol and in Isopropyl Alcohol at Difperent Temperatures.
(Muchin, 1913, see also Timofeiew, 1894.)
Grains Cdli per xoo Girnms Sat. Solution in: '
• •
CEuaa.
CiHiOH.
OH1OH.
OHiOHCiio).
0
67
33 S
16
36 -9
5
• • «
41
22
36.9
10
68
54 (MttlJS'mtt.tmp.)
28.5
37-2
30
69
S3
41.5 (tctemp.)
37-3
25
69s
52.2
37-8
37-3
30
70
s^-s
3SS
37-3
40
71
50.8
345
37-3
SO
725
so
34 0
37-3
Solubility op Cadmium Iodide in Ethyl Ether. (Linebaiger, 1895)
M Mds Cdls per Cms. Cdls per
* ' zoo Mols. CdIs+(CtEb)^. zoo gms. (.OB^^,
o 0.03 0.148
15.5 0.04 0.198
20.3 0.05 0.247
Solubility op Cadmium Iodide in Methyl Formate, Ethyl Formate, Propyl
Formate and in^Ethyl Acetate at Different Temperatures. (Mudun, 1913.)
f.
13.0
26.0
Gms. Cdls per xoo Gms. Sat. Solution in:
kcOOCHs.
0.84
0.7s
0.66
HCOOCtHs.
I ..,16
1.05
0.77
HCOOC1H7.
2.37
2.07
I. S3
CHsCOOCiHi.
4.73(?)
1.67
2.02
Solubility of Cadmium Iodide in Aniline, Pyridine and in Quinolinb at
Different Temperatures. (Mudun, Z9Z3.)
r.
40
SO
60
70
80
90
100
Gms. Cdls per xoo Gms. Sat. Solution in:
CeHiNHs.
1.7
2.3
31
4
S-i
6.4
8.4
OHiN.
...
0.1
o-S
1-7
4.8
13 -4
30
CBiIJ.
2
3S
S
6.7
8.3
Solubility of Cadmium Iodide in Mixtures of Solvents at Different
Temperatures. (Muchin, X9X5.)
Comporition of Solvent
in Mols.
iCH,0H+2CHCl,
iCHiOH+iCHCU
iC^0H+2CHCI,
iCiH»OH+iCHCl»
2C,H»0H+iCHCl,
xCAOH+yCHCU
<t
(t
iCAOH+iCeH«
2CA0H+iCeH«
aCaOH+^rCiHe
Wt. per cent
Alcohol in
Solvent.
II. 8
21. 1
16.2
27.8
435
60.3
91S
22.8
371
S4I
9.8
Gms. Cdit per xoo Gms. Sat. Solution at:
o*.
II. O
22.4
7.S
139
25.2
34-4
4S-4
17.6
26.1
33 -S
6.S
x6.8'.
10.4
22.3
71
14.3
24.1
9-3
20.6
6.6
13 -6
16.3 (16.3")
26.0(15.7°)
3S.3(iS^)
lS-2 (31.2^)
26.0
((
• • •
177 G4ikiiniii maam
SoLUBiLirr OP GAufniii Iodidb m MixmBS op Solvbhts^
OwMoL
P^rniMHO
teM«LCUi
>
Qw Mat. I>jndia»40M MdL
t-Tini
Gb
r.
IS. Cdlipcr
xoo Obs.
r.
no Gas.
GM-OUilNt
«*.
too CtCttk
Sftt.SoL
Sftt-SoL
Sa.SoL
S»I.Sok.
so. I
1.27
63
6.3
57.9
1.77
7a.S
32.6
54
1,72
64
8.3
60
a. a
74.0
3S 9
56
2.3
64s
".3S
65
4. a
76
363
58
30
64
Z4.8
70
8.1
80
40.8
60
4.0
6a
22.0
71
"•5
85
41.6
62
5-6
61.15
24.67
71.5
15.0
90-4
4« 67
SOLUBIUTT OP CADmUM lODIDB IN EtHYL EtHBR CoNTAININQ WaTBB AT I2\
Gms. HjOper
100 gms. ether +^>~» 0.0 o.io 0.30 0.50 0.70 0.90 x. 00 x«io x.X4aat
Gms. Cdlsper
100 gms. solvent-^ 0.1430.78 2.07 3.36 4.77 6.467.30 8«a7 8.68
DisTRiBunoN OP Cadmium Iodidb at 30* Bbtwbbn:
OMtt and Datter, 19x30
Water and Amyl Alcohol. Water and Ethyl Ether.
Gms. per xoo oc. ^ Gms. per xoo cc. ^
H^ Uyer (c). Akobol Layer (c*). ^'
47-75 43 I"
29.08 25.86 I. 13
14.46 12.55 I. 15
10.69 ^*94 1-20
6.23 4.94 1.33
2.42 1.S4 1.55
1.93 I. 10 1.76
1.76 0.94 1.87
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures:
Cadmium Iodide + Cuprous Iodide (Rernnaan, 1911.)
" '' + Mercuric Iodide (Saadonnini, 1914.)
" " + Potassium Iodide (Bxand, 191 aO
" " + Sodium Iodide
CADMIUM AMMONIUM I0DIDI8 (Mono and Di).
Solubility of Each Sbparatbly in Water, etc.
(Rimbach, 1905; Eder, 1876.)
Cd. Mono Ammonium Iodide. Cd. Diammonium Iodide.
Gms. CdIfl.NHJ per Omi. CdIi.iNH4l par
Solvent t*. 100 pms. t». too Omi.
fa^ Layer (c).
Ether Layer (c*).
?•
37 18
8.38
4-43
30.03
6.61
4. 54
15.38
309
4-97
12.60
a. 38
Sa9
9.89
1.83
5 40
7.68
1.06
S5»
4 03
0.73
5.60
3.10
0.51
6.03
Solution.
Solvent.
Solution.
Solvent
Water
IS
52.6
Ill
US
85-97
6x1. 6
Abs. Alcohol
IS
53
"3
IS
59
143
Abs. Ether
IS
29.4
41-7
IS
10
IZ
CADMIUM I0DIDI8
178
CADMIUM POTASSIUM I0DIDI8, Mono - CdIs.KI.iW>,
Di = CdI,.2KI.2H,0,
CADMIUM DiSODIUM IODIDE CdIi.2NaI.6H^.
^ SoLUBiUTT or Each Separately in Water, srCt at is\
CBda.)
Cms. CdIt.KI Gms. Cdlf.aKI Gma. CdIt.aNai
per 100 Gms. per 100 Cms. per 100 .Gma.
» ^ / * »
Solvent. Solution. Solirent.
Sohent«
Soltttka.
Water 51.5
Abs. Alcohol . . .
Abs. Ether
Solvent*
106
Sobdaa.
57 -8
41-7
3-9
137
71
41
Solution.
61.3
53-7
9.0
158-8
116. 2
9.9
CADMIUM HITBATS Cd(NO,),.
Solubility in Water.
(Funk — WisB. Abh. p. t. Rdduuistalt 3 440, W^
»•.
Gms. Cd(NQa)t
pa 100 Gms.
Mols. CdCNCMt
per 100 Mols. H^.
SflKd
PhMe.
SdutioD.
Water.
-13
— 1
+ I
0
+18
37-37
47-33
52 -73
52.37
55-9
59-67
89.86
III. 5
109.7
126.8
4-55
6.8s
8.50
8.37
9.61
Cd(N0,),.9H,0
Cd(N0A.4H,0
30
58-4
140.4
10.7
it
40
59-5
61.42
76.54
159-2
326 -3
12. 1
25.0
U
Density of saturated solution at i8° = 1.776.
The eutectic of the system Cd(NOi)i.4HiO + Cd(NOi)i is at!44.8* and has the
composition Cd(NOt)i.2.65HsO. (Vuilev, 19x0)
CADMIUM OXALATE CdC,0«.3H^.
I liter of sat. aqueous solution contains 0.033 S™. CdCiOi at I8^ (Kohhamch, Z908O
<vui Doortcr; X910-ZX.)
CADMIUM SILICATE CdSiO..
Fusion-point data are given for CdSiOt + ZnSiOt.
OADMIUM SULPHATE CdSO^.
Solubility in Water.
^ylios and Funk — W. Abh. p. t. Rdchanstalt 3> 444t 'oo; see also Kohnstamm and Cohn ~^ Wied
Ann. 65* 344i '98; Steinwehr — Ann. der Phys. (Drude) [4] 9, 1050. 'oa; Etard-— Ann. diim. phyi
[7J a 536, '94)
t\
Gms. CdS04
per 100 Gms.
Solid
Phase.
f.
Gms. CdS04
per xoo Gms.
Solution. Water.
Solid
Phase.
Sdudon. Water.
-17
44.5 80.2
CdS04.7H,0
40
43.99
78.54
CdS04.iH,0
— 10
46.1 85.5
a
60
44.99
83.68
tt
- 5
48.5 94.2
u
73.5
46.6
87.28
tt
-18
43.35 76.52
CdS04.fH,0
74.5
46.7
87.62
CdS04.H,0
— 10
43.27 76.28
tt
77
42.2
73.02
tt
0
43.01 76.48
u
85
39.6
65.57
tt
.fio
43. x8 76.00
u
90
38.7
^3-^3
u
20
43.37 76.60
tt
100
37.8
60.77
M
For results at high pressures, see Cohen (1909).
179
CADMIUM SULFATl
Solubility of Cadmium Sulphate in Aqueous Solutions of Sul-
phuric Acid at o*.
(Encd^Compt. rend. 104* 507, 'S?.)
EquTuents pv
10 Gms. HsO.
CdSO«.
Density
ofSdtttiaos.
^ranuH/).
H|SO«.
' HaSO«.
CdSO*.
0.
71.6
1.609
COO
74.61
387
70.9
I 591
1.90
73 87
12.6
6a ^4
I 545
6.l8
65 03
38.1
50. 6
1.476
13-78
52-73
43-3
40.8
I -435
ai.23
42 52
47.6
37 0
1. 421
23-34
38-56
53-8
32-7
1.407
26.38
3407
71-5
23 0
1-379
35 06
23.96
100 gnu. 95% formic acid dissolve 0.06 gm. CdSOi at 18.5^ ' (Aachtn, 1913.)
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
CdS04 + LiaSOi, CdSOi + K1SO4 and CdSOi + NatSOi by Calcagni and Marotta
(1913).
Solubility of Mixed Crystals of Cadmium Sulphate and Ferrous
Sulphate in Water at 25**.
(Stortenbecker — Z. phyiik. Chem. 34. 109, '00.)
CompositioD of Solution.
Mol. percentCdin
Gms. per xoo Gms. HaO. Mob. per xoo Mob. HaO.
CdS04. FeSO«.
CrraUb with sf Mob. H3O.
76.02 0.0
57.61 10.63
Crratsb with 7 Mob. HsO.
57.61 10.63
26.69
Cd.
6.57
4.98
Fe.
0.0
1.26
4.98 1.26
0.0
3-165
Mol. % Cd. A??^ <^
in Sol.
100
79.8
79.8
78.5
44.6
24.4
0.0
Solid Phase.
100
99-0
36.6
34-6
II. I
4.8
0.0
CADMIUM POTASSIUM SULFATE CdKs(SO«)i.
Solubility in Water.
(Wyrouboff, 1901.)
*•• ^2*S2^^ SoBdPW.
V.
"i^^^"" 3oIidPh«.
16 42.89 CdK«(S04)i.2l^O
26
42.50 CdKi(S04ViiIW3
31 46-82
31
42.80 "
40 47 .40 "
40
43-45 ;;
64
44.90
GADBOUM SODIUM SULFATE i8o
CADMIUM SODIUM SULFATE CdNai(S04}t.2H^.
mm
Solubility in Water, also with the Addition op Caduivu Sul-
phate AND OP Sodium Sulphate.
(Koppd, Giimpery — Z. physik. Chem. 52* 413, '05.)
24
30
40
O
10
20
40
14.8 40
o 37
CdSO«
22
22
22
40
39
40
39
10
20
as
30
35
40
32
22
16
9
8
. ner loo Gms.
Soluttoo.
Na^SOt'
07
29
65
8S
34
16
18
60
S3
69
71
83
80
35
a?
•as
^5-
■SS
^S-
.89
IS
•32
4-
.91
5-
.36
5-
.89
7-
.18
4-
•30
6.
•S3
8.
.69
14.
•33
19.
.31
37.
.36
29.
.98
38.
Cms.
per I
gjO.
CdSO*. nSoT
100 Cms. Mob. per xoo Mob.
H|0.
CdSO«. NaaSO«.
Solid PhMB.
35-49
36.28
37 24
73-54
72.77
73 81
7538
72.68
66.32
55-34
36 .25
25.60
14.62
13 26
16.24
24
24
25
8
9
9
13
8
II
14
23
31
44
47
46
04
60
45
85
55
45
56
3^
62
78
52
06
14
06
27
3-07
3-14
3-22
6.36
6.30
6-39
6.52
6.29
5-74
4-79
3-14
2.21
1.26
I-I5
1. 41
3
3
■
3
I
I
I
I
I
I
I
2
3
4
5
5
CdNa,(S04),.2H,0
CdNa,(S0J,.2H,0
+ C(iSO/.fH,0
CdNa,(S0Ja.2H,0
-fNa3SO^.iol4o
CdNaa(S0J,.2H,0
CADMIUM SULFIDE CdS.
1000 cc. HiO dissolves 9 X io~* gms. CdS at i8^
(Weigel, 1906.)
OAESIUM ALUMS
Solubility op Caesium Chromium Alum, Caesium Iron Alum,
Caesium Indium Alum, and op Caesium Vanadium Alum in
Water.
(Locke — Am. Ch. J. a?* 1741 '01.)
Fomrab of Alum.
CsjCr3(SOJ^.24H,0
tt
ii
Cs,Fe3(SOj4.24HaO
u
ii
i\
CSjIn,(SOJ^.24HaO
CsjV,(SOJ,.24H,0
Cms. per xoo cc. H^O.
»•.
Anhydrous
Hydrated'
Salt.
Salt.
as
0.57
0.94
30
0.96
I 52
3S
1.206
1. 91
40
1-53
2.43
25
1. 71
2.72
30
2.52
4 01
3S
3-75
6.01
40
6.04
9.80
25
7-57
"•73
25
0.771
I 31
GnmMbb. Salt
xoo cc. HjP.
O.OOI5I
0-0025
0.0032
0.00405
0.004S
0.0066
0.0099
0.0156
00172
0-00204
See also Alums, p. 53.
I8l
GAXSIUM CBLOBAUBATl
GAS8IUM OHLORAUBATB CsAuCU.
GmBbCsAnCk
V, per xoo Gms.
Solutkn.
lO o.s
30 1.7
Solubility in Watbr.
(Rosenbladt, i88d.)
Gms.CsAaCI«
f. per xoo Gm. f.
SohitioiL
40 3.2 80
SO 5-4 90
60 8.2 100
70 12.0
Giiis.CiAaO<
per zooGmu
Sniiirinn
i<5.3
21.7
27s
QAESIDM FLUOBOBIDI CsBFU.
icx) grains water cUssolve 0.92 gram CsBFU at 20% and 0.04 gram at loo^
(Godeffzpy, Z876O
:i:*9
CsBr.
Solubility of Caesium and Lead Bromides and their Double Salts
IN Water at 25**.
• (Foote, 1907.)
GmSb per loo Gms. Sat. SoL
Gms. per xoo Gms. Sat. Sol.
CsBr.
PbBn.
« outun x-uBsc
; CsBr.
PbBn.
■% ouua raamem
0.24
0-33
PbBr,+CsPb,Br6
33-65
trace
CsPbBrs
033
0.36
« ((
36.7
«
" +rs«PbBn
12.83
trace
CsPbjBrs
46.4
ct
Cs^PbBr.
17.24
u
It
51.15
it
m
U
17.68
«
" +CsPbBrs
54.4
ta
" +CsBr
18.58
(1
CsPbBrs
55 23
0
CsBr
GAXSIUM Mercuric BBOMIDX C8Br.2HgBrt.
100 grams saturated aqueous solution contain 0.807 gram CsBr.2HgBri at i6^
(Wells, zSga.)
CAESIUM GABBONATB CssCO..
100 grams absolute alcohol dissolve 11. i grams CsiCOt at 19% and 20.1 grams
at b. pt. (Bumen.)
GAXSIUM BiGABBONATX CsHCO,.
100 grams sat. solution in HiiO contain 67.8 grams CsHCQi at about 20'.
(de Forcxaud, 1909^
GAXSIUM GHLORATX CsClO, GAXSIUM PerGHLORATX CsClOi.
Solubility of Each in Water.
(CabolarU x9ia; see also Carlson, xgio.)
Results for CsClOs.
Results for CSCIO4.
r.
Gais.CBaOi
per xoo Gms.
HsO.
V.
Gms. CsClOi
per xoo Gms.
HiO.
f.
Gms. CsaO«
per xoo Gms.
HiO.
— •
Gms. CsCIO«
f. per xoo Gms.
0
10
2.46
3.8
50
60
19.4
26.2
0
10
0.8
I.O
50 5.4
60 7.3
20
25
6.2
7.6
70
80
34-7
45.0
20
25
1.6
2.6 (rf=
70 9.8
i.oi) 80 14. 4((2= 1.084)
30
95
90
58.0
30
2.6
90 20.5
40
13-8
ICO
79.0
40
4.0
zoo 30.0
CAESIUM GHLORIDS
182
OASSIUM OHLOBIDE CsCl.
Solubility in Watbr.
OBeifcdey — Ttana. Roy. Soc. (Loud.) 203 A, ao8, '04; see also Hinrichsen and Saduel — Z. phyak.
Chem. 50, 99. 'o4-'o5: at af, Foote.)
G. CsCl per xoo Gms.
O
10
20
40
50
Solutiaa.
61.7
63.6
65.1
66. 4
67 S
68.6
Water.
161 .4
174.7
186.5
197 -3
308.0
218.5
G.Mol.CBa
per Liter.
6.74
7. II
7 38
7 63
7.86
8.07
G.CsaperiooGms. G. Mol. CsQ
60
70
80
90
100
II9.4
S^ution
69.7
70.6
71.4
72.3
73 o
74-4
Water.
239.7
239 S
350.0
360.1
370.5
290.0
per Liter.
8.38
8.46
8.64
8.80
8.96
9.33
Gms. per xoo Gms.
Solution.
SoUd Phase.
ScLUBiLiTir pp Mixtures op Caesium Chloride and' MerciTric 'Chloride
IN Water at 25''. (Foote, Z9Q3.)
Gms. per xoo Gms.
Soludon.
dscE
38.63
17.03
1.53
0.61
CsCL
65.61
65.78
62.36
57.01
52.35
51-08
49-30
45-95
4523
HgOs.
0.0
0.215
0.32
0.64
1.23
1.44
1.49
Z.69
1.73
csa
CsQ + CiiHsClc
Double Salt
CasUgOf
= 65.1% CsQ
CaAClc + CflsHgClA
Double Salt
CatHgCU = ss-A%CaCL
C8|H«CU + CsHgOt
0.49
0.40
0.44
0.41
0.25
0.18
0.0
HgCli.
1.32
0.51
0.42
2.64
2
3
4.63
4.68
5.65
7.09
6.90
SoUd
Double Salt
csQaa«=38^«aa
r.91 )
1.78 J
}
CsHs +CsHgsCl.
Double Salt
CsHgaae = 93.7%CBa
CsHgtOe + CsHgsQu
Double Salt
c&Hbau= xx.i%Csa
CsHgBQu + HsOt
HgO,
SOLUBILITT OF MIXTURES OF CaESIUM ChLORIDE AND MERCURIC CHLORIDE IN
Acetone at 25**. (Foote, 19x1.)
Gms. per xoo Gms. Solution.
Gms. per zoo Gms. Solution.
Solid Phase.
CsCl
Mixed salts
CsCl. HgCUt.
0.032 o
o.ii 0.02
0.19 0.16
0.25 0.17
0.45 13.08 CsCLHgCli
0.46 21.50
0.56 27.2
it
it
CsQ.
0.48
0.48
0.47
0.32
0.20
0.13
+CsC1.2HgCli 0.0
28.48 CsC1.2HgCl2
39.65 "
44.40 " +CsC1.5HgCli
49.83 CsC1.5HgCI,
57.74 "
57.76 « +HgCl,
57.74 HgCli
CAESIUM Iridium CHLORIDES CsiIrCU, etc.
100 gms. H|0 dissolve o.oi i gm. caesium chloroiridate, Cs2lrCUat 19^ (Delepine, 1908.)
100 " " " 0.05 gm. caesium hexachIoroiridite,C^IrCl6.^HiO at 19^
100 ." " " 0.83 " caesium aquopentachloroiridite,|Cs2H|0IrClf at 19'.
CAESIUM Platinic CHLORIDE CsPtCU.
100 gms. HsO dissolve 0. 1 35 gm. CsPtCU at 20^. (Rosenheim and Weinheber, 1910-zz.)
CAESIUM Tellurium CHLORIDE CsTeCU.
Solubility in Aqueous Hydrochloric Acid. (Wheeler. 1893.)
100 parts HCl (Sp. Gr. 1.2) dissolve 0.05 part CsTeCU at 22*.
100 parts HCl (Sp. Gr. 1.05) dissolve 0.78 part CsTeCU at 22*.
CAESIUM Thallium CHLORIDE 3CsCl.TlCk.2H2O.
100 parts HaO dissolve 2.76 parts 3CsCl.TlCl3.2HtO at 17% and 33.3 parts at
I00^ iGoddboy, 18864
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 (SandoDnini and Scaipa, 19x3; Sandonnini, 19x4.)
+ Silver Chloride
+ Thallium Chloride « « «
+ Lithium Chloride (Koneng, 19x5; Richards and Meldium, X917O
+ " " +NaCl (Richards and Mddnim, X917.)
+. Potassium Chloride (Zemcznaiy and Rambach. 19x0.)
+ Rubidium
+ Sodium
II
II
II
II
II
II
II
II
II
II
M
CAESIUM CHROMATES, CsiCr04, CstCr^, etc
S(H.UBiLiTY IN Water at 30'.
(SchreinemakoB and Mdjeringh, 1908.)
Cms. per xoo Gms.
Gms. per ]
[oo Gms. Sat.
Sat. Sol.
Solid Phase.
1
Sol.
SoHdFlaie.
Carf).
CrO^ '
Cs«0.
CtOi.
70.63
0.0
CsOH.nH,0
0.169
21.21
CstCrAo
69.22
O.II9
" +CstCr04
; 0.096
25 -59
it
36.06
1.883
Cs8Cr04
1.89
36.19
ti
31.00
7-523
s<
2.79
41.68
it
31-68
9.652
u
3.29
44.23
it
35.80
13.08
ii
±3-13
±44. 45
"+Ca,CiAt
31 OS
10.79
CsfCrjOr
2.96
44.66
CsiCrtOu
24.05
8.98
C(
3.40
46.03
a
3.04
2.16
ii
3-94
56-77
it
1. 61
4.57
"+CsiCrAo4.3S
62.70
" +C1Q1
1. 18
7.95
CsjCrAo
2.33
62.50
CiO»
0.586
15-05
ti
0
62.28
n
CAESIUM FLUORIDE CsF.i}HiO.
100 gms. H2O dissolve 366.5 gms. CsF at 18°, solid phase CsF.i}HiO.
(de Fonaand, X911O
CAESIUM H7DB0XIDE CsOH.
100 gms. sat. solution in HiO contain 79.41 gms. CsOH at 15^ (de Forcrandt
1909a); for 30", see above.
CAESIUM lODATE CsIOi.
100 parts HsO dissolve 2.6 parts CsIOs at 24^ and 2.5 parts 2CsI0t.Ii0f at
21^ (Wheeler, 189a; Barker, 1908O
CAESIUM Per lODATE CSIO4.
loogms.H20di8Solve2.i5gms.CsI04at I5^dJ^8at. solution -1. 0166. (Baiker,i9o8.)
CAESIUM IODIDES Csl, Csit, etc.
Solubility in Water at 25".
(Foote and Chalker, 1908.)
im. per loo Un
3s. bat. Solution.
Empirical Comp.
of Residue.
Present in Residue.
OL
L
7.72
1. 18
Csl8 29
Csis and Csis
7.69
1. 19
Cslsw
ti it
3.40
1.23
Csl5:75
Csl6 and I
2-3S
1.23
Csl7.«
« it
2-39
1-25
Csli9.s
ft C(
CAESIUM lODIDI
184
OAEtlUK IODIDE Csl.
Solubility op Mixtures op Caesium Iodide and Iodine in Water.
(Foote — Am. Ch. J. ag» azo, '03.)
-4
-4
-4
—0.2
Cms. per 100 Gms.
Solution.
^ 1
Csl.
27.68
27.52
0.85
52.2
52.2
52.2
52.2
73
73
73
0.0
0.09
0.31
0.34
Gnu. per zoo Gms.
Solution.
T.
452
3 36
3-3^
3-45
15 07
10.50
4.08
Csl.
16.7s
6.69
6.72
6.65
26.98
16.66
6.27
Gms. Der zoo Gms.
solution.
35-6
35 -6
35-6
35-6
Csl.
51.48
51,66
10.72
3-74
I.
0.0
0.71
1.78
1.60
In Separated Heavy Solution
Gms. per 100 Gms. Solution.
'"m: — '
22.94
22.80
• « •
27.56
17.68
73
74
68
80
72
63
40
02
Solid Phase at
both Temps.
Csl
Csl and Csl,
Csl, and Csl,
Csl, and I
Solid
Phase.
Csl, and Csl,
Csl, and I
Csl,
I
Csl, and Csl,
Csl,
I
OAESIUK (Tri) IODIDE Csl,.
100 cc. saturated aqueous caesium iodide (about 17 per cent Csl)
solution contain 0.97 gram Csl, at 20°, density of solution « 1.154.
(Wells— Am. J. Sd. [3] 44, aai, ^pa^
OABSIUM NITRATE CsNO,.
Solubility in Water.
(Berkeley — Ttans. Roy. Soc. (Lond.) 203 A, 9x3, '04.)
Gms. CsNOs per
G. Mob.
Gms. CsNOi per
t».
zoo
Gms.
CsNOa
per liter.
t».
zoo Gms.
G. Mols CsNOt
per Liter.
Solution.
Water.
Solution. Walrrl
0
8 54
9 33
0.476
60
45.6 83.8
3 41
10
12.97
14.9
0.725
70
51.7 107.0
4.10
20
18.7
23 0
I. II
80
57-3 134.0
4.81
30
25-3
33-9
1.58
90
62.0 163.0
5 50
40
32.1
47.2
2.12
100
66.3 197 0
6.19
so
39a
64.4
2-73
106.2
68.8 220.3
6.58
The Ice Curves for Mixtures of Caesium Nitrate and Water,
Determined by the Synthetic Method.
(Jones, 1908.)
Supersolubility curve.
Solubility curve.
r of Ciystslli. Gms. CsN(>|,i)er
zation. '^
-0.3
—0.4
— 1.2
-"1-3
— 1.4 (Eutec.)
100 Gms. HJO.
0.21
1.28
6.01
8.0
Solid
Phase.
Ice
a
u
it
t* of CiTstalli- Gms. CsNQi oer
100 Gms. HiO.
(sation.
— 1.2
-2.5
-3.0
-3-2
-3-2
0.21
1.28
3-99
6.01
8
SoUd
Phase.
Ice
(I
€1
€$
The eutectic is given as -1.254* and 8.51 gms. CsNOs per 100 gms. H|0, by
Washburn and Maclnnes (191 1).
185
CAE8IUM~^OXAL2lTE
CAESIUM OXALATE C8iCiO«.HiO.
Solubility of Mixtukes of Caesium Oxalate and Oxalic Acid in Water
AT 25**.
CFoote 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. Solntiop.
BflCsO«. OsCiOi.
10
G. Mob. per 100
G. Mob. HjO.
HiCsO«.
^ao*.
Solid
Phue.
10
7
4
4
4
4
4
4
3
I
o
o
o
o
o
.29
• •
0.
.90
9^
.11
25 •
•33
.27
27.
28.
.40
.8a
35-
40.
•45
•OS
.04
42.
48.
68.
.91
71-
•77
73-
•75
74-
•74
75-
.0
75-
61
92
12
55
30
90
10
32
80
69
24
45
04
20
82
2.274
2.314
1.924
1. 162
1.279
1.267
1.476
1-752
1.672
1.268
0.688
0.648
0.598
0.596
0.625
0.0
o
o
I
2
2
3
3
4
5
II
13
14
14
15
IS
1
035
614 1
81 )
06
14
07
71
OS
16
56
06
51
0
93
97
1
HaC,0^.2HaO
H^Q04.2HaO+I^Cs(C,OJ,.2H,0
Double Salt.
H3Cs(Ca04),.2H20
H3Cs(QO,)32H,0+H.Cs,(QOJ,
Double Salt.
H,Cs,(QOJ,
H,Cs3(QOJ,+HCsC30,
Double Salt.
HCsQO^
HCsC,04+H,Cs.(C30J,
Double Salt.
HeCSeCQOJy
HeCs8(C,04)7+ Cs,C,0,.H,0
CsjCjO^-HaO
CAESIUM Telluradd OXALATE Csi[H6Te08.C>04l.
100 gms. HiO dissolve 6.42 gms. Cs2[H«TeO«.C|04] at o**, 12.39 gms. at 20%
15.08 gms. at 30"", 19.78 gms. at 40"" and 27.66 gms. at 50"".
(Roacaoheim and Weinbieber, X9Z0-ZZ.)
OAESIUM PEBMANQANATE CsMnO,.
100 CO. sat. aqueous solution contain 0.097 gm. CsMnO^ at i®, 0.23
gm. at 19^ and 1.25 gms. at 59^ (Pwtonoo— J.Am.Chem.Soca8i I73S. '•^^
OAESIUM SELENATE CsaSeO^.
100 grams H,0 dissolve 245 grams CssSeO^ at 12®.
(Tuttoa — J. Chem. Sec. 7ii 850i '97^
OAESIUM SULPHATE Cs^SO^.
Solubility in Watbr.
CBerkeley — 'naiu. Roy. Soc. (Loud.) 303 A, axo, '04.)
O
10
20
30
40
SO
Gms. Cfl9S04 per
100 Gms.
SolutioQ. Wattf.
62.6 167. I
63 -4
64.1
64.8
65 -5
66.1
173 I
178.7
184. 1
189.9
194.9
G.Mob.
CsiSO*
per liter.
3 42
3-49
3 56
3 62
3-68
3-73
60
70
80
90
100
108.6
Gms. C8aSO« per
TOO Gms.
Water.
199.9
205.0
210.3
214.9
220.3
324.5
Solution.
66.7
67.2
67.8
68.3
68.8
69.2
G.Moli,
CssSp.
per Liter.
3 78
3-88
3 93
3-97
4-00
Gnu. Azihydroos Sdt
per zoo Gms.
Gm. Mob.
Salt per 100
Solution.
Watrr. '
Gma.HsO.
S8-i6
139 -9
0.24SS
29.52
31 -49
41.9
46.0
0.081
0.0882
50.29
lOI.I
0.1967
34-77
4458
53-3
80.4
O.II06
O.IS7
20.37
27.87
25.6
38.6
0.0495
0.0738
CAESIUM DOUBLE SULTATEi 186
Solubility op Caesium Doublb Sulphates in Water at 25®.
(Locke — Am. Ch. J. 37t 459i '01.)
Name. Fonaula.
Caesium Cadmium Sulphate CHCd(so«)s^H^
Caesium Cobalt Sulphate Cs^CoCSOJaJSH^
Caesium Copper Sulphate c^Cu(SO«)s^HaO
Caesium Iron Sulphate CatFeCSOJa^HaO
Caesium Magnesium Sulphate CaaMcCsoja^HaO
Caesium Manganese Sulphate CsaBinCSOJa^HaO
Caesium Nickel Sulphate CsaNi(so<)aj6H30
Caesium Zinc Sulphate CiACSOja^HaO.
SoLUBiLnT OF Caesium Sodium Sulfates in Water at aj*.
(Footet 19x1.)
Gma. per 100 Gms. Sat. Solution. Per cent CaSOi Empirical Compoaition oC
CteSOi. NaaSOi. inReaidue. « pRoidue.
54.65 11.44 89.98 iNa«S04.3.53Cs2S04
54.58 11.63 78.22 iNa«S04.i.4iCsfS04
54.81 11.25 34 67 4.8Na«S04.iCstS04
The author's solubility method for determination of the formation and com-
position of double salts b described in the paper containing.the above results.
CAESIUM DihydroxyTABTEATE CsiC«H408.2HsO.
100 gms. HtO dissolve 22.5 gms. CsiC4H40s.2HsO at 0^ (Fentoo, 189&)
CAFFEINE CiH(CH,),N40,.H,0.
Solubility in Water.
(Avenge cwve from reaulta of Zalai, 19x0; Pellini, 19x0, and U.S.P., Sth Ed.)
«• Gma. CiH(CHi)j^40» ^ Gma. CiH(CH|)«N40|
^' per xoo Gma. HiO. *' per xoo Gma. HiO.
o 0.6 40 4.64
IS 10 50 6.7s
20 1.46 60 9.7
25 2.13 70 13.5
30 2.8 80 19*23
Solubility of Caffeine in Organic Solvents.
**-'• *•• S^oi^^S^SiJ^ Solvit.
Ethyl Alcohol 35 1.33(2) Carbon Tetia-
« ti
35 1.33(3) Carbon Tetia- C 18
35 1.88(1) chloride < 30
60 5.85(1) 'b.pt.
Methyl " 35 1.14(2) Chloroform 17
Amyl " 35 0.50 (3) (d. -0,810) " 35 13.3
Amyl Acetate 30.5 0.73 (3) (dbi -0.86a) " 35 11.92
Acetic Add (995%) 31.5 2.6 (3) " b.pt. 15.63
Acetone 30.5 3.33 (3) (<bi -0.83a) Ether 18 o.z3
Aniline 30.5 29.4(3)(At-xx)8o) " 35 0.37
Benzaldehyde 30.5 i3.x(3)((bi-xx)87) " b.pt 0.30
Benzene 18.0 0.91(4) Trichlorethylene 15 0.76
^2) Dichlorethylene 15 1.82(7)
3)((fci-o.87s) Pyridkie 30-35 34-39(8)
b.pt. 5 . 39 (4) 50% Aq. Pyridine " 11 . 12 (8)
Carbon Disulfide 17 0.06(5) Toluene 35 o.58(3)(iH-o.86x)
Xylene 32.5 i . 13 (3)(*i-o.847)
(i) - U. S. P.; (2) - Schaefer, 1913; (3) - Seidell. 1907; (4) - GiSckel, 1898; (5) <- Commaille, 1875;
(6) — Gori, 1913; (7) — Wester and Bruins (1914); (8) — Dehn, 19x7.
Data for the solubility of caffeine in mixtures of alcohol and chlcM'oform and
alcohol and benzene are given by Schaefer (1913).
«
187
CAFFEINE
Solubility op Caffeine in Aqueous
Vice Versa.
Results at 25^.
Gms. per xoo Gms. HsO.
CsHmNiOi.
2.13
8.32
38.10
51-74
46.27
24.79
9-47
o
CrHcOiNa.
O
6.67
4S
76.7s
76.68
69 56
62.97
61.17
Solid Phase.
C«H»N40i.HsO
Solutions of Sodium Benzoate and
(Pellini, 19x0.)
Results at 40°.
Gms. per 100 Gms. HiO.
CSH10K4O1.
(»
((
"+C7Hi0iNa.Hs0
C7H«0feNa.Hs0
<(
K
M
4.64
31 -43
56.82
57-99
55-98
18.31
o
CTHcOiNa.
O
2531
69.68
74.64
74.02
67.97
59.82
Solid Phase.
CaHioN40i.HsO
(f
"+C7Hi0«Na.Hj0
CrHtOiNa-HiO
(f
<f
Solubility of Caffeine in Aqueous Solutions of Sodium Salicylate and
Vice Versa. (P^lUni and Amadori, 19x2.)
Results at 25*
Gms. per lop Gms. H^.
C«HioN40i.
2.13
38.36
55-23
74.32
16.78
13.22
9-03
o
CrHiOsNa.
O
30.76
47.31
68.81
124.96
121.27
120.54
"5-43
Solid Phase.
C«Hk»N40i.H^
Results at 40®.
Gms. per 100 Gms. HiO.
CgHioN^Oi.
It
u
It
OrHiOfeNa
«4
((
tt
4.64
59-49
86.49
95-94
26.93
10-75
o
C7HfO>Na.
O
37-47
62.47
69.15
131-52
124.35
119.66
Solid Phase.
C<H]oN40i.HiO
tt
If
((
CrHiOiNa
tt
u
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, X914.)
Grams Caffeine in:
- *
xos cc. HiO Layer. 50 cc. CHCIa Layer.
0.0090 0.0563
0.0180 0.1048
0.0291 0.1770
Ratio of Caffeine in
Equal Vols. HiO and CHCIs.
0.0456
0.0492
0.0470
CALCIUM ACETATE Ca(CH,C00),.2H,0.
Solubility in Water. (Lumsden. 1903; Krasnicki, 1887.)
Gmg. WlCB^COGh
Gms. Ca(CH^OO)s
*•.
per 100 Gms. Solid Phase.
t».
per xoo
Solution.
Oms.
Wate^.
SoUdPfaaae.
^lutioxi. Water.
0
27-2 37.4 CaCCHsCOOsjHgO
60
24.6
327
Ca(CH8COO)j.aHaO
10
26.5 36.0 Ca(CH,COO)ijHjO
80
25.1
33-5
Ca(CH3C00)a.aH,0
20
25 -8 34.7 Ca(CHaCOO)ajHaO
84
25 -3
33'^
Ca(CH8COO)a.2H80
25
255 34 • 2 . Ca(CH8COO)j.aHaO
85
24.7
32.9
Ca(CHsCOO),.H,0
30
25 -3 33-8 Ca(CH«C00)2.aH,0
90
23 -7
311
Ca(CH3COO)aJIaO
40
24 -9 33 2 Ca(CH,COO)8.aH20
100
22.9
29.7
Ca(CHsCOO)8.HaO
Solubilitt of Calcium Acetate in an Aqueous Saturated Solution of
Sugar at 31.25**. (Kshier, 1897.)
100 gms. solution contain 8.29 gms. CaCCHgCOO)! + 60.12 gms. sugar.
100 gms. water dissolve 26.3 gms. CaCCHsCOO)^ + 190.3 gms. sugar.
100 oc anhydrous hydrazine dissolve i gm. calcium acetate at room temp.
(Welsh and Broderson, 19x5.)
GALGIUM ACETATIS
i88
OALOIUM (Tn) Methyl AOETATE Ca[(CH,},CCOO],.
OALOIUM (Di) Ethyl AOETATE Ca[(C,Ha)aCHCOO],.
OALOIUM Methyl Ethyl AOETATE Ca[CH,(C,H,).CHCOO],.
Solubility op Each in Water.
(Lanikn — Momtfah. Chem. 14, 7x7, '93; Keppish — /Mi. 9, 600, '88; Sedlitzki ~ iluf. S, 573, '87.)
Ca, Tri Methyl Acetate. Ca. Di Ethyl Acetate. Ca. Methyl EthyL
Acetate.
Gnu. Ca(CcHM)s
Gms. Ca(C6HuOt)s
GmB. Ca(CBH^02)t
!•.
per TOO
Gms.
per xoo Gms.
per xoo Gms.
Water. Solution'.
^ater.
Solution.
Water.
Solutiab.
0
7 30
6.81
30 -3
23.22
28.78
22.35
10
6.84
6.40
27.8
21-75
31-71
24.07
20
6.54
6.14
25.6
20.38
33-7^
25 23
30
6.40
6.01
23 -7
19.16
34 92
25.89
40
6.44
6.05
22.1
18.10
35 20
26.04
SO
6.64
6.22
20.8
17.22
34.60
25-71
60
6.86
6.42
19.9
16.60
33"
24.89
70
7. II
6.64
19.2
16. II
30. 74
23.41
80
733
6.87
• ■ ■
• • ■
27.49
21.56
OALOIUM Methyl Propyl AOETATE Ca[CH,(C,H,).CHCOO],.
OALOIUM (Di) Propyl AOETATE Ca[(C,H,),CHCOO],.
OALOIUM (ISO) Butyl AOETATE Ca[(CH3),CH(CH,),C00],.
Solubility op Each in Water.
(Stiassny — Monatsh. Chem. xa* 596* Vt Furth — Ihid. 9, 3x3, '88; K6nig — Ihid. z& sa, '94O
Ca. Methyl Propyl Acetate. Ca. Di Propyl Acetate. Ca. Iso Butyl
Acetate.
Gms. Ca(C6HiiOa)s
per xoo Gms.
Gms. CaCCsHttfO^
per xoo Gms.
Gms. Ca(C6HiiOs)fl
per 100 Gms.
Water.
Solution.
Water.
Solution.
'Water.
Solutkn^
0
16.58
14.22
9-57
8.73
7.48
6.96
10
15-80
13-65
8-35
7.71
6.38
S-99
20
ISU
J315
7.19
6.71
5-66
s-36
30
14.61
12.7s
6. II
s-77
S-3I
5 04
40
14.31
12 45
509
4.84
S-3I
5 -04
SO
13-94
12.24
4.14
3-98
5-68
S-37
60
13-79
12.13
325
3-^5
6.41
6.03
70
13-78
12.12
2.44
2.38
7-Si
6.n8
80
13.89
12.20
1.65
1.63
8-97
8.23
90
• • •
...
■ • •
• • ■
10.79
9-74
CALCIUM BENZOATE Ca(C«H.COO),.
1 00 cc. sat. solution in water contain 3 .02 gms. Ca [CeHf COO]i at 26^. (de Jong, 191 a.)
100 gms. sat. solution in water contain 8.6 gms. CaLCsHeCOOls at 15*^ and 10.2
gms. at 100**. (Tarugi and Checchi, 1901.)
CALCIUM BOBATES CaB/)«4HsO, CaB«04.6HsO.
SoLUBiLmr OF Each Separately in Water.
(Mandelbaum, 1909.)
' Gms. per 100 Gms. Sat. S<d.
f.
70
90
BsOs. CaB40«.
0.0365 0.310
0.036 0.307
0.048 0.392
0.0315 0.310
Solid Phase.
CaBiO«.4H^
(amorphous)
Gms. per xoo Gms. Sat. Sol.
ff
(4
M
30
50
70
90
BfOt.
0.0205
0.032
0.068
0.067s
CaBflOi.
0.254
0.353
0.457
0-359
Solid Phase.
CaBi0«.6Hii0
" (cryit.)
i89 CALCIUM BOBATE
SOLUBILITT OF CAI/HUM BORATES IN AqUEOUS SOLUTIONS OF BORIQ ACID
AT 30**.
(Sboigi, 1913.)
Omft. per xoo Gi
OS. Sat. Sol.
SoUd
Phase.
Gms.perxooijii
ns. Sat. SOL
Solid
B^
CaO.
Bid.
CaO.
Phaae.
0.014
0.126
Ca(0H)t
0.869
0.067
3.3.9
0.032
0.140
If
1. 116
0.076
M
0.098
0.194
<f
1-339
0.093
" +Z.3.U
0.127
0.217
« +1.1.6
2.058
0.093
Z.3.I2
0.134
0.220
Z.1.6
2.509
0.099
tt
0.138
O.II^i
ft
2.730
O.III
M
0.162
0.106
CI
3.732
0.325
M
0.166
0.107
" +a.3.9
2.798
0.109
«
0.171
0.109
tt It
3-313
0.143
M
0.290
0.052
2.3.9
3.841
0.-I52
M
0.610
0.054
ii
4.250
0.15s
«* +HiBOfc
0.767
0.059
u
4.179
0.137
HaBOk
I.I
.6 = CaO.B,Oi.6HiO,
2.3.9 = 2CaO.3B1Qs.9HtO,
1.3.12 = Ca0.3BjOi.i2H,0.
Many determinations, in addition to the above, are given in the original paper.
CALCIUM BBOIODB CaBr,.6H,0.
Solubility in Watek.
CKremeis, 1858; ' Etaid,''i894, gives results whkh yield an irregular curve and are evidently kss Mrnialu
than those of Kremecs.)
Gms. CaBn per
Gms. CaBn per
f . .
100 Gms.
Solid Phase.
V.
xoo
Gms.
Solid Phase.
Water.
Solution.^
Water.
Solution^
-22*
lOI
50.5
CaBn.6HaO+Ioe
34-
2t
i8S
65.1
CaBn.6Hk0+CaBiMH^
0
"S
555
CaBn.6Ha0
40
213
68.1
CaBxMHiO
10
132
57
It
60
278
73-5
M
20
143
58.8
fC
80
29s
74.7
M
25
153
60.5
u
105
312
7S-7
«
• 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 Ruif^and Plato, 1903.
CALCIUM PerBBOlODE CaBr«.
Data for the formation of calcium perbromide in aqueous solutions at 25^
are given by Herz and Bulla (191 1). The experiments were made by adding
bromine to aqueous solutions of CaBrs and agitating with carbon tetrachloride.
From the bromine content of the CCI4 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 CCI4. This furnishes the necessary data for calculating the
amount of ^calcium perbromide existing in the aqueous layer.
CALCIUM BUTY&ATS 190
OALOIUM (Normal) BUTTBATE Ca[CH,(CH,),COO],.H,0.
OALOIUM
(ISO) BUTTBATB Ca[(CH,),CH.COO],.sH,0.
Solubility op Each in Watbr.
(Lnmaclen — J. Chem. Soc. 8x, 355, 'oa; see also Chancel and Parmender — Compt. rend. Z04* 494,
'87; Deszathy — Monatsh. Chem. 14, 351, '93, and also Hecht — liebig's Annalen 3x3, 7a, '8a, gi^e
results for the Dormal salt which are somewhat below those of Lumaden for the lower temperatures.
Sedlitzki — Mooatah. Chem. 8» 566, '87, gives slightly different results f or the iso salt.)
Calcitixn Normal But3rrate.
Cms. Ca(C«H70i)9
•, per iqo Gms.
l^ater. Soluticn!
Calcitmi Iso Butyrate.
Gms. Ca(C«H7Qi)s
per 100 Gms.
Water.
Solid
Phase.
O
10
20
25
30
40
60
80
zoo
30
19
18
16
IS
IS
•31
•IS
16.
16.
■ 20
IS-
.72
IS-
•25
14.
.40
14.
•IS
13-
•9S
•8S
13-
13-
89
08
39
OS
71
09
16
01
69
o
20
30
40
60
62
6s
80
100
20.10
22.40
23.80
25.28
28.40
28.70
28.25
27.00
26.10
Solution.
16.78 Ca(C^IL0j),.sH|O
18.30 *'
19 23
20.65
22.12
a
it
St
ti
22.30
22.03 Ca(C^HyO,),.H,0
21.26
20.69 "
CALCIUM d CAMPHORATE CuHM04Ca.7HsO.
Solubility of Calcium Camphorate in Aqueous Solutions of Camphoric
Acid at 15** and Vice Versa.
(Jungfleisch and Landrieu, 1914.)
Gms. per zoo Gms. Sat. Sol.
Gms. per 100 Gms. Sat. Sol.
C«Hu(C0OH;t. LKiHMO«Ca.
1.3s I 23
1-57 1-97
I. 71 2.5s
2.18 4.34
2.33 4-73
Solid Phase.
CsHii(C00H)t
M
f(
U
«•
CbHuCCOOH)!. CioHuOiCa.
2.90 7.7s
3 8.66
307 8.57
1.50 7.94
Solid Phase.
CtHu(C00H)a
" +Ci|HiiOft.Ca.7EbO
C|ftHiiOiCa.7H^
If
If
o 7-37
Calcium camphorate tetrahydrate exists at higher temperatures. Its solu-
bility at 100^ was found to be 8.68 ems. CioHmO^Qi per 100 ems. sat. solution.
By careful work, the result at 15° for CioHi^4Ca.4HsO was found to be 12.21
gms. CioHi404Ca per 100 gms. sat. solution.
CALCIUM CAPBOATE (Hexoate) Ca[CH,(CH,)4C001,.H,0.
CALCIUM 3 Methyl PBNTANATE Ca[CH,.CH,.CH(CH,)CH,.COO]i.3HsO.
CALCIUM CAPBYLATE Ca[CH,(CHs)«COO],.HsO.
Solubility of Each in Water.
(Lumsden; the Pentanate, Kuhsh, 1893; see also Keppish, x888, and Altschul, 1896,
for results on the Caproate.)
Ca. Caproate.
M Gms. CaCCJIuO^t per
*^' 100 Gms. Rfi.
o 2.23
20 2.18
40 2.15
50 2 . 10
60 2.15
80 2.30
100 2.57
Ca. 3 Methyl Pentanate. Ca. Caprylate.
Gms. Ca(C<Hii0»)t per 100 Gms. Qms. CaCCgHuO^t per
Water.
".33
17.18
18.99
18.73
17.71
13-37
9.94
Solution.
10.98
14.66
IS -97
15.78
1S.04
11.80
9.04
xoo Gms. HiO.
0.33
0.31
0.28
0.26
0.24
0.32
0.50
I9X
CALCIUM CARBONATC
GALdUM CARBONATE CaCQi.
EgUILIBKIUlf IN THE SYSTEM CaO-H20-COj AT l6*.
The following data for the solubility of calcite (CaCOi) in water at i6^ in con-
tact with air containing the partial pressure P of COi were calculated from the
results of Schloesing (1872). Engel (1888), and others by Johnston (191^) and
Johnston and Williamson (1916I. These authors describe the changes in the
system resulting from a gradual increase in partial pressure of CQi, as follows:
"We begin by considering the equilibrium between the hydroxide M(OH)s and the aqueous
solution saturated with it as affected by a progressive increase from zero of the partial pressure
P of COi in the atmosphere in contact with the solution. Addition of COi is foUowed by a dis-
tribution between the vapor and liquid phases until there is equilibrium between the residual
partial pressiuv of COi and the HsCCH in solution, and in turn between the latter and the
several ions; the net effect of this is a definite decrease in [OH"], the concentration of hydroxide
km, which necessitates that more of the hy(hoxide dissolve in order to keep the solubility-
product [M++][Oir~]* constant. Consequently the total concentration of M-H- 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 b a determination of
M, whereas it would decrease if one should determine [OH~p. This process continues until
the product niif*H-][COi"] reaches the value requisite for the precipitation of MCOi (on the
assumption- that superaaturation 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 solubilitv (as measured by the total [M]) begins to diminish, because increase of
P increases [CCH^] while the product [M'H-KCOi"] must remain constant so long lu MCXDi is
the stable solid phase; this increase of [CQiT] continues until a definite pressure Po is reached,
when the formation of bicarbonate in the solution becomes the predominant reaction and
[CQir] begins to decrease again. Po is thus a minimum in the solubility curve. With
further increase beyond Po the concentration of both M-H- and HCOs increases steadily
untfl the precipitation value of the product [M++)[HCOi'~)' is reached at Pi, which is a transi-
tion pressure at which both carbonate and bicarbonate are present as stable solid phases.
Beyond P% bicarbonate alone is stable, and its total solubility falb off very slowly with
further increaae of partial pressure of COb."
The Calcxtlated Ion-Concentrations and Solubh^ity op Calcite in
Water at 16*^ in Contact with Air Containing the Partial Pressure
P OF COi.
1^^ Grams
Partial PreKuxe P
of COi Measured
in Atmospheres.
Ion-concentrations per Liter X lo"^.
Ca++.
0H-.
COI-.
HCOr.
3.16X1O-"
138.5
277
0.0071
0.0000235
2.80X10-1®
6.81
13.3
0.144
O.OI
9.78XIO-*
2.377
3.82
0.414
O.IO
6.14X10-*
1.654
1.82
O.S93
0.30.
2.19X10-^
1.476
1.02
0.665
0.60
3.73X10-^
1-459
0.787
0.672
0.787
3.85X10-^
1-459
0.774
0.672
0.80
6.07X10""^
1-473
0.614
0.666
I
7.62X10"*
2.051
0.147
0.478
3
7.63Xio-»
3.777
0.034
0.260
7
2.15X10"^
S-I97
0.0174
0.188
10
2 Xio"^
5-09
0.0182
0.19
9.96
2.5 Xio"^
5-46
0.0157
0.18
10.54
3 Xio-^
579
0.0140
0.17
11.22
35 Xio-^
6.08
0.0126
0.16
11.82
4 Xio"^
6.35
o.oiis
0.16
12.36
4.5 X10-*
6.59
0.0107
0.15
12.86
5 X10-*
6.82
O.OIOO
0.14
13-32
Liter
Xio-*.
Liter.
• • •
2
0.074
0.026
0.018
0.016
0.0159
0.0159
0.016
0.022
0.040
0.056
5S2
0.055
S-93
0.059
6.31
0.063
6.64
0.066
6.94
0.069
7.21
0.072
7-^
^6
0.07s
CALCIUM CARBONATE
192
The Solubility of Calcium Carbonate (Calcite) in Water at i6* in
Contact with Air Containing Partial Pressure P of COi.
(Gale, from Schloesing, 1872, and Engel, x888, by Johnston, 19x5.)
Total Ca, Mob. Total Ca(HC0i)s ^*S^J rJ?1S^ Total Ca.MoU.ToUl Ca(HC0^,
Atmospheres.
0.4167
Partial Pressure
Pof COiin
Atmospheres.
0.000504
0.000808
0.00333
o.. 01387
0.02820
0.05008
0.1422
02538
per Liter.
0.000746
0.000850
0.001372
0.002231
0.002965
0.003600
0.005330
0.006634
Mols. per Liter.
0.000731
0.000837
0.001364
0.002226
0.002961
0.003597
0.005328
0.006632
0.5533
0.7297
0.9841
I
2
4
6
per Liter.
0.007825
0.008855
0.00972
0.01086
0.01085
O.OI4II
0.01834
0.02139
Mols. per Liter
0.007874
0.008854
0.00972
0.01086
0.01085
O.OI4II
0.01834
0.02139
The Solubility of Calcium CarbonatbI (Calcite) in Water at 25° in
Contact with COi Under Increasing Pressures. (McCoy and Smith, 19x1.)
Approz. Pres-
sure of COi in
Atmospheres.*
O.I
I.I
9.9
13-2
16.3
25
cm
Mols. per Liter Sat. Solution.
HsCOi.
0.003522
0.03728
0.3329
0.444
0.550
0.858
Cms. per Liter Sat. Sol.
CaCHCO.),.
0.0041 16
0.009734
0.02236
0.02495
0.02600
0.02603
HiCOi.
0.22
2.3
20.6
27s
34-1
alson
CaCHCOi)!.
0.67
1.58
3.62
4.04
4.21
4.22
SoUd Phase.
CaCQs
ti
u
u
Ca(HCQ,)i
tt
* Calc by Henry's Law from COi concentrations. See also remarks under Ferrous Bicarbonate, p. 336.
These results show that the solution becomes saturated with Ca(HCOs)s at
about 15 atmospheres pressure of COi, and it would be theoretically possible to
convert all the CaCOi to Ca(HCC)i)i bv introducing sufficient COa at pressures
l^eater 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 COs at one at-
mosphere pressure was found by Cavazzi (1016) to be 1.56 gms. CaCOa at 0°
and 1. 1 752 gms. at 15°. A supersaturated solution prepared by passing a rapid
stream of COi through sat. C^(OH)i solution at 15*^ contained 2.29 gms. CaCOi.
Solubility of Calcium Carbonate in Water at 15*. (TreadwcU and Renter, 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, z888; Ander-
son, 1888-89; Engel, x888; Lubavin, 1892; PoUacci, 1896.)
cc COs per 100 cc.
Gaseous Phase
(o*and76onmi.).
8.94
Partial Pressure
of COi in mm.
Hg.
67.9
6.04
45-9
5-45
2.18
41.4
16.6
1.89
14.4
1.72
131
0.79
6
0.41
31
0.25
0.08
1.9
0.6
Gms. per
xoo cc. Saturated Solution.
4,
FrceCOi.
Ca(HCOi)».
Ca.
0.1574
0.1872
0.0462
0.0863
0.175s
0.0433
0.0528
0.1597
0.0394
0.0485
0.1540
0.0380
0.0347
0.1492
0.0368
0.0243
O.I33I
0.0329
O.OI4S
0.1249
0.0308
0.0047
0.0821
0.0203
0.0029
0.0595
0.0147
• • ■
0.0402
0.0099
■ • •
0.0385
C.OO95
Therefore i liter sat. solution at 15* and o partial pressure of COj contains
0.385 gram Ca(HCO|)i. Determinations similar to tne above, made in o.i »
NaCl solutions at 15", are also given. It is pointed out by Johnston (1915)1 that
although Treadwell and Renter 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 CABBONATE
Solubility of Calcium Carbonate (Calcitb) in Water in Contact
WITH Air at Different Temperatures. *
(Wells. 191S.)
(Jopiin, Mo., caldte 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 COi content of the air varied from ^.02 to 3.27 parts per 10,000.
The calcium content of the solutions was detemuned by titrating with 0.02 n
NaHSO^, using methyl orange as indicator. The solutions were slightly acid
to phenolphthaleine, showingithat the calcium was present chiefly as bicarbonate.)
0
Cms. CaCOi per liter.
0.081
10
20
25
0.070
0.06s
0.056 (0.046)
30
0.052
40
SO
0.044
0.038 (0.029)
Results in parentheses by Kendall (19 12). In connection with these it is
stat^ by Johnston (191 5), that assurance is wanting that the partial pressure of
COi was the same at both temperatures and the results are, therefore, not neces-
sarily comparable.
SOLUBILITT OF CAIXIUlk CARBONATE IN WaTER AT DIFFERENT TEMPERATURES
AND IN Contact with Air Containing Different Partial Pressures or
CO,.
(Leather and Sen, 1909.)
Results at i<
> •
Results at 25*.
Results at 40"*.
Partial
Pressure
Gms. per
Liter Sol.
Partial
Pressure
COiinGas
Phase.
Gms. per
CaCOi.
Liter Sol.
COi.
Partial
Pressure
COiinGas
Phase.
Gms. per
> CaCOi.
Liter Sol.
COiinGas
Phase.
CaCOi.
COi.
COS. ^
0.8
0.193
O.II7
0.7
0.159
0.091
0.6
0.136
0.078
i-S
0.193
0.152
1.6
0.177
O.III
1.7
0.143
0.085
1-7
0.238
0.13s
4.6
0.341
0.208
2.9
0.17s
0.106
6.8
0.44s
0.327
7.8
0.446
0.301
35
0.232
0.169
9.9
0.627
0.456
16.5
0.539
0.522
7
0.284
0.234
13.6
0.723
0.560
30.1
0.743
O.7IS
14.9
0.384
0.293
14.6
0.686
0.623
3SS
0.7SS
0.803
22.2
0.427
0 333
316
1.050
1. 117
317
0.480
0.476
Similar results also given for 20®, 50* and 35®.
The mixtures were constantly agitated at constant temperature. The solid
phase in each case was found to be CaCOs and it is concluded that Ca(HCOi)s
cannot exist in this solid state above 15^.
In discussing the experiments of Leather and Sen, Johnston (1Q15) points
out that their method of analysis gives low results for CO*. A calculation of
the data yields verv irr^^lar 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 0.5X10"* at 40^
Data for the solubility of CaCOs m 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' tnat small
amounts of CaCU, CbSOa or NaHCOs did not affect the solubility-product con-
stant. Small amounts of NaCl, NasSOi and MgS04, containing no ion in common
with CaCOk, resulted in an increase of the total calcium in the solution.
Data for tlie solubility of calcium carbonate in water, determined by the con-
ductivity method, are given by Holleman and by Kohlrausch and Rose (1893).
CALCIUM CABBONATB 194
Solubility of Calcium Carbonate in Aqueous Solutions of Ammonium
Chloride.
Results at 1 2"-! 8*^. Results at 2^**. Results at 60° for Calcite and Aragonite.
(Cantoniaad Goguclia, 1905.) (Rinddl. i9xo5 (Waiynaki and Kouropatwinaka.
(Flasks allowed to stand (Constant agitation 1916.)
98 days.) . ^24brs.),..
Gms. per Liter Sat. SoL ■ Gms. per Liter SaL Sol.' dms. lyr Liter. Gms. per Liter.
NH4CI. CaCOi. ' NH4CI. CaCO.. NH4CL Calcite. NHiCl. Aragonite.
53.5 0.423 6.7 0.285 O 0.028 O 0.041
100 0.609 '3-4 0-373 i-oy 0.164 i-o? 0.184
200 0.645 26.8 0.502 5.35 0.333 5.35 0.371
"" 53-5 0.678 10.70 0.453 1070 0-505
26.76 0.664 26.76 0.728
5352 0.934 5352 i.ois
160.56 X.2I X60.56 1.36
Solubility of Calcium Carbonate in Aqueous Solutions of Ammonium
Nitrate and of Triammonium Citrate.
InAq. NH4N0sat 18°. InAq.NH4NO»at25^ In Aq. Triammonium Citrate at 25^
(BerjuandlKoeminiko, 1904.) (RIndell, 1910.)
Gms. per Liter Sat. Sol. Gms. per Liter Sat. Sol.
l>fH*NO». ' CaCO». ■ NH4NO.. CaCOa. '
o 0.131 5 0.200
5 0.2II 10 0.278
10 0.258 20 0.383
20 0.340 40 0.526
40 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. (EUert and Hempei, 191a.)
Aq.Salt *o drSld^'t ^'SFS' Aq. Salt 4. <SSd^t 2.?*;^^
Solution. * • per x^Gms. I-,^^,- SoUon. * ' ^^ x^ P-^,^-^
MgCls.6HsO 5 o 2.337 NaCl 5 50 3 -740
5 6.1 2.352 " 5 86 3.783
" 5 50 3404 " 5 106.9 3690
" 5 86.9 4083 " 5 175.6 3.350
" 5 350 3-301 " 5 263.4 2. 811
" 5 700 2.736 " 8 351-2 2.163
" 5 "50 2.205 MgS04.7HjO 14 105.3 2.177
" 5 1725 1.706 " 14 (sat.) 0.914
*' 5 2300 sat. 1.406 NaiSO^.ioHsO 14 137 -7 1.406
NaCl 5 28 3.280 " 14 (sat.) 1.920
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:
T« ^^««^o^ «,;*u ,:^ In contact with i »„ ^^„^^^ -^t, ^' In contact with i
In contact with air. atmosphere of CO,. ^" ^^"^^ ^'^** ^"^- atmosphere of CO,.
(Rindell. 19x0.)
Mols. Citrate
per Liter.
C;ms. Ca(X)i
per Liter.
0.0625
0.125
0.250
0.500
1.492
2.264
3.980
6.687
Gms. per loo Gms.
Gms. pe
r 100 Gms.
Gms. per 100 Gms.
Gms. per
100 Gms.
Sat.
Sol.
Sl
t. Sol.
^t.
Sol.
Sat.
K«SO«
Sol.
KCI.
CaCOi.
KCI.
CaCOa.
KtSO*.
CaCOi.
CaO.
0
0.0013
0
0.062
1.60
0.0104
0.69
0.69
3-9
0.0078
3-9
O.I4S
315
O.OI16
1-37
0.69
7.23
0.0078
723
0.150
4.73
0.0132
1.67
0.47*
13.82
0.0072
13.82
0.165
6.06
0.0148
2.18
0.30*
18.21
0.0070
18.21
0.154
8.88
0.0192
2.99
0.24*
26
0.0060
26
0.126
10.48
0.0188
* Solid 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 8^- aragonite
at 60*^. (Warynaki and Kouropatwinaka, 19x6^
195
CALCIUM CABBONATB
SOLUBILITT OF CaLCIUM CaRBONATB IN AqUEOUS SOLUTIONS OF SODIUII
Chloridb at 25°.
Solutions in contact with.
COi Free Air.
(Cameron, Bell and Robinson, 1907.)
Cms. per 100 Gma. HsO.
Ordinary Air. COi at One Atmos. Pressure.
(Cameron and Seidell, 1902.) (Cameron, Bell and Robinson, 1907.)
Gma. per xoo cc. Sat. Sol.
Gma. per 100 Gma. HiO.
NaQ.
CaCO^
NaCL
CaCOi.
' NaO.
CaCOi.
1.60
0.0079
I
O.OII2
1.49
0.150
S.18
0.0086
4
0.0140
569
0.160
9.2s
0.0094
8
0.0137
11.06
0.174
11.48
0.0104
10
0.0134
15.83
0.172
16.66
0.0106
IS
O.OII9
19.62
0.159
22.04
o.oiis
20
0.0106
29.89
0.123
30.50
0.0II9
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 CQi are
given by Cameron, Bell and Robinson (1907).
Data for solubility of CaCOi 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 2$\sLTe ^ven 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 COs, 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 S™^. NaCl dissolves 0.071 gm.
aragonite at 60 .
(Warynaki and Kouropatwinaka, 1916.)
Solubility of Calcium Carbonate in Aqueous Solutions of Sodium
Hydkoxidb in Contact with COx Free Ais.
(LeBlanc and Novotny, 1906.)
Solvent.
At i8\
At 9S*-xod*.
Water
0.0128
0.0207
About o.oooi n NaOH
0.0087
0.0096
" o.ooion "
0.0042
0.0069
" o.oioon "
0.0042
0.0057
Data on the equilibrium in aqueous solutions of CaCOi, NatCOi and NaOH
are given by Wegscheider and Walter (1907).
Solubility of Calcium Carbonate in^Aqueous.Solutions of Sodium Sulfate.
Solutions in contact with:
COi Free Air at 25*.
((Cameron, Bell and Robinaon, 1907.)
Gms. per 100 Gms. HsO.
Ordinary Air at 24^
(Cameron and Seidell, 1903.)
Gma. Total Ca
NaaSOt.
0.97
I
4
12
14
19
23
65
90
69
55
3S
90
CaCOa.
O.OI51
0.0180
0.0262
0.0313
0.0322
0.0346
0.0360
Gms. NaaSOi
per Liter.
5
10
20
40
80
150
250
per Liter Calc
a8Ca(HC0^i.
0.175
0.232
0.277
0.332
0.400
0.510
0.725
Freezing-point data for mixtures of calcium carbonate and calcium chloride
are given by Sackur (1911-12).
CALCIUM CHLOBATl
196
CALCIUM CHLORATE Ca(C10,)i.2H,0.
100 grams saturated aqueous solution oootain 64 grains Ca(C108)t at 18^.
Density of solution is 1.729. (MyUus and Funk, X897.)
CALOIVM OHLOBIDB Cad,.
Solubility in Water
(RooKboom — Z. phvrik. Chem. j« 43, tSo; lee alio Mulder; Ditte — Compt. rend. 9a» 94a, '81; Engd
— Aim. cfaim. pbjrac. C6JX3. 381, '88; Euid — Ibid, [7] a, 53a> 'm-)
Density of saturated solution at o" - 1.367, at 15^ " i*399f at 18^ ■■ 1417;
at 25' - 147.
Solubility of Calcium Chloride in Aqueous Solutions of Hydrochloric
Acid at o".
(Engd, 1887.)
CaCU.
HCl.
d^ of Sat. Sol.
CaOt.
HCl.
d^ of Sat. Sol.
51.45
0
1.367
29.84
15.84
1.283
46.45
3.32
1-344
20.12
23.15
1.250
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, 191 2.)
f.
CaOt.
Mgcb:
Solid Phase.
16.7
41.2
31.6
Mgai.6H^-|>CaC]a.6Hi0
21.9s
57.1
26
+Tadihydrite
28.2
54.5
28.4
Tachhydiite+MgCli.6Hi0
116.7
0
85.63
+ " +MgCli4HiO
25
32.3
17.9
+CaCls.6HsO+Caai.4HiO
28.2
80.1
16. 1
+CaCl».4HiO
28.2
88.7
7.24
CaC]a.6HgO+Caas.4HiO
Tachhydrate - 2MgClt.CaClt.i2HiO.
100 grams H|0 dissolve 63.5 grams CaClj + 4.9 grams KCl at 7° (M).
100 grams HiO dissolve 57.6 grams CaClj -j- 2.4 grams NaCl at 4® (M).
100 grams HjO dissolve 59.5 grams CaClt -j- 4.6 grams NaCl at 7** (M).
too grams H|0 dissolve 72.6 grams CaCls + 16 grams NaCl at 15*^ (R).
(M) - Mulder. (R) - Rftdorff.
Gma. CaOt per
Gma. Cadi per
t«.
100 (
Gras. goM
♦•.
xoo i
Water. Solutian. *"""*
Water.
-55
42.5
2^.8 Ice + COi-fiHgO
60
136.8
jy.g CaClt.aHsO
-2S
50.0
33'
^ CaasJdHaO
70
141. 7
58.6 Caaa.aHjO
0 .
59-5
37'
^ CaQt^HsO
80
147 0
-Q - CaCla.aHsO
10
65.0
39'
4 CaQt^dHiO
90
152-7
5o.5 CaCl,.aH,0
20
74. 5
42,
J Cadt^HsO
100
159.0
61 .4 CaCla.aH,0
30. 2
102.7
SO.
7 CaCl|j6HsO
120
173.0
63.4 Caa,.aH,0
20
91.0
47
6 CaOa^iOc
140
191 0
65.6 Caa,jHgO
29.8
100.6
SO
I -»H,0«+iiH^
z6o
222.5
5p.O CaCl,.aH^
40
"5 3
S3
.4 .4H|0«.
170
255.0
71 .8 CaClj.aH«0
20
104.5
SI
.1 Caaj.4Hi0^
175.5 297.0
M. QfCaat-aHflO
74.O(+CaClt.ili0
29.2
IZ2.8
53
.0 w|H|0^+j6H|0
180
300.0
75.0 CaClaHiO
3S
122.5
SS
.0 w|Hso^
200
3II.O
75.7 CaCI«.HgO
38.4 127. s
56
.0 4HsO^+Caat.9Hg0
235
332 0
76.8 CaCIa.HaO
45-3
130-2
S6
.6 4HsOa + CaCla.aHiO
260
347 0
77.6 CaOiJIjO
197 CALCIUM CHLOBmS
Solubility op Calcium Chlokidb in Aqueous Solutions op Sodium
Chloride at 25* and Vice Versa.
(Cameron, Bell and Robinson, 1907.)
rf|- Gaa. per 100 Gms. HiO. Solid
Sat."l. CaOi. Naa. ?»"««.
84 O CaCls.6Hi0
1. 4441 78.49 1.846 " +Naa
1.3651 58-48 1.637 NaCl
1.3463 53.47 1.799
1.2831 36.80 7.77
(f
Sat.^L
Gms. per xoo
Gms. H«0.
Solid
CaCU.
NaCl.
Phase.
1.2653
30.08
10.70
Naa
1.2367
19-53
18.85
(4
1.2080
3.92
32.48
fl
z . 2030
0
35.80
It
Solubility of Calcium Chloride in Aqueous Alcohol at Room Temperature.
(BOdtker, 1897.)
Vol. Gms. Vol. Gms.
Solution Used. Per Cent CaCIsper Solution Used. Per Cent CaCbpex
Alcohol. 5 cc. SoL AlcohoL . 5 cc. SoL
15 Gms. CaClt.6HiO 15 Gms. CaClt.6HjO+20 cc.:
+ 20 cc. alcohol 92.3 1.430 alcohol -h 2 Gms, CaCls 99.3 1.561
15 Gms. CaCli.6H,0 " + 3 " " 993 1590
-h 20 cc. alcohol 97.3 1.409 " 4-4 " " .99-3 1-641
15 Gms. CaCl,.6HaO " +5 " " 993 i-709
+ 20 cc. alcohol 99 . 3 z . 429
Z5 Gms. CaCl».6HjO
-h 20 cc. alcohol
4- 1 Gm. CaCU 99.3 z.529
Solubility of Calcium Chloride in Aqueous Solutions of Acetone
AT 20**.
(Frankforter and Cohen, 19x4.)
Measured amounts of acetone were added to known solutions of CaCh 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
CaCls 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 icp Gms. Sat. Sol. Gms. per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer.
Acetone. CaCIs.
9 40.5* ) (solid phase
22.7 38.i6tJ CaCW
20.8 31.2
20.2 28
21 24.4
23 2Z . z
25 19 . 2
30 15-6
35 12.8
40 Z0.5
45 8.8
50 7.4
55 6.1
60 5
65 3.9
70 2.8
75 1.8
80 z
85 0.5
90 0.2
95 o.z
* Pomt on solubility curve, f Qvuulniple point. 40
Acetone.
CaClt.
Acetone.
Carii.
90.2
0
.186
28.5
16. 6z
83.3
0
.628
34.6
"97
8z
0
.948
40
10.6
78.5
I
.321
43-5
936
60
5
(plait point)
60
5
Points on
the Binodal Curve at Different
Temperatures.
f.
Gms. per xoo Gms. Sat. Sol.
Acetone.
CaCl,.
5
31.09
15 52
23.64
zo
22.77
Z5
31 09
15.52
18
30.58
15.27
25
2Z.44
22.25
25
29 83
14.89
30
20.99
21.79
30
29.27
Z4.62
35
2Z.14
20. 9z
35
28.59
14.29
40
19-83
20.58
point. 40
27.90
13.93
CALCtDM CHLOBIDK 19S
SOLUBILtTY OF CaLCIUU CSLORIDB IN A SATURATED SotmOIt OV SUGAR AT
100 grama saturated solution contain 43.84 grams sugar + 2<i.3^ grams CaCli,
or 100 grams water dissolve 135.1 grams sugar + 79.9 grams CaCIf
100 gms. 95% formic acid dissolve 43.1 gms. CaCli at 19°. (A«eh»o, 1911O
100 cc. anhydrous hydrazine dissolve 16 gms. CaCli at room temp.
(WeUh ud^iodenoD. ,9,5.)
100 gms. propyl alcohol dissolve 10.75 E">b. CaCli (temp.?). (SchUmp, 1894.)
CaCl,+CaF, (1) (2)
CaCli+Cal, (I)
CaCl,+CaO(3)
CaCl,+CaSia {4)
CaCl,+CaSO.(3)
CaCl,+CuCl (5)
(i) - RuS aod Plito, 1U13: <
-Uuw, laii; (6)- SiDdonni
nog, 1914; (10) — Schmefer, ign
CALCIDH CSLORIDK AOITAHIDATB Caa,.3CH,C0NH,.
- Pl»to. 1901; (j) - SMtiii, isu-is; (4) - KiiMdedf, 1910: (j)
r I9'i; (?) ~ Sudonnim, 1913; <S) — Suidooiuiu. 191J; (9)— Eo^
SOLUBH.ITY IN ACETAUIDB .
T Varioits Tem^raturbs, Detbruined b
Synthetic Method.
(MestdiiitUD. 1908.)
Gnu. per loo Gum.
SoUd « S^. Sol. So
•■ '^■S&">)
-CCl,.
Pbue.
•• '•&&«=
(-CO.
PhMB.
82 m. pt. 0
0
CHKX)NH.
100 65.6
25.3
J
78 8
31
"
ISO 70s
17.1
74 IS -4
5 9
"
i6s 74.8
s8.8
66 27
10.4
'■
175 80.6
31
54 39-2
151
"
.80 8s, s
32.9
46 Eutec. 45
17 3
" +1.6
184 90,5
34.8
58 48.5
18.7
1.6
186 ti.pt 94. s
36-4
'+c»cw?)
62 54- S
21
!oo 97. s
37-5
CCM?)
64 tr. pt. 62 . 1
23-9
..6+.,3
38. S
1.6 - CaCl,.6CH.CONHt
1.3 - CaCi,.3CH,CONH,.
CALCIUM CHLORIDE ACETIC ACIDATE CaClt.4CHiCOOH.
Solubility in Acetic Acid at Various Temferaturbs, Detbruined by the
Synthetic Mbthod,
(MEUctiutkin, 1906.)
Gnu. per too Gnu. Gnu. per tea Gnu.
„ S«t. Sol. Solid „ Sat. Sol. Solid
■ "^MF
-CO. "-■
■^ajOT
-CCh.
6.3 m. pt.
0
0 CH.COOH
40
54. 7
■7.3
S
18
5-7 "
4S
63
19
9
4
27
8.5 ■
SO
69. s
9
3
34
10.7 ■
60
79S
«S
I
I.I Eutec
4«
133 ■•+'-•
65
84-S
16
7
0
47.6
IS '^
70
91.2
28
8
S
SO
1S.8 -
73 HI. pt.
100
31
6
14 - CaCWCHiCOOH.
199 CALCIUM CHLORIDE
CALCIUM CHLOBIDS ALCOHOLATES CaCaCHsOH, CaC^.3CH»0H.
(The compounds were prepared by mixing anhydrous CaCis with the alcohbf.
In the case of the methyl alcohol compound, the tri CHtOH salt crystallizes
above 55**, the tetra salt below this temperature.)
Solubility of Each in the Rbspbctive Alcohol at Various Tbm peraturbs.
Determined by the Synthetic Method.
(Menschutkin, 1906.)
Results for CaClt-sCHtOH. Results for CaCls.aCiHfOH.
Gms.per
xooGms.
Gms. per 100 Cms.
Sat. Sol.
Gms. per xoo
Gms.
Sol.
Solid
Phase.
f.
SoUd
Phaae.
f.
Sat. Sol.
CaCIi.3CHsOH-CaC1,.
CaCkaCHiOH-Caai.
CaCh^CiHiOH
-CaClft
0 33.3
17.85
1*4
95
66.3
35-5
1.3
0
34.8
15. 5
10 37.6
20.15
"5
70.3
37
6
20
46
20.5
20 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 52
27.8
165
86.2
46
2
70
80.8
36
50 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*
100
53
6
90
91.9
40.8
55 60.S
32.4
" +1-3
190
■ • •
55
7
x.i(?)
^K
96.2
42.8
75 63.1
33.8
1.3
215
■ • •
57
7
«f
97*
100
44. 5
• M. pt.
14 e CaCla4CHtOH. 1.3 = CaCli-aCHiOH, i.i - CaCls.CH«OH.
OALOXUM OHBOMATE CaCiO«.
Solubility op the Several Hydrates in Water.
(Mylius and Wrochem — Wias. Abh. p. t. Reichanstalt 3, 46a, '00.)
^» Gms. CaCr04 per 100 Gms. Mols. CaCrO* Oms. CaCrO* per 100 Gms. Mds.CaCrp*
Water. SoluUcn. HtO. Water. Solutkn. H^)*
Solid Phase. « CaCrO«.3HsO. (Mooodinic.) SoUd Phase, CaCrO«.iH«0.
o 17.3 14.75 20 o 7.3 6.S 0.84
18 16.68 14.3 1.93 z8 4.8 4.4 0.51
20 16.6 14.22 1.93 31 3.84 3.7 0.44
30 16.5 13.89 1.85 38.5 2.67 2.6 0.31
45 14.3 12.53 1.65 SO 1.63 1.6 0.19
Solid Phase, fi CaCrO«.sHsO (Rhombic.) 60 I . I3 I.I O . I3
o 10.9 9.8 1.25 ICO o.Ci 0.8 0.09
l3 II. 5 10.3 1.33 Solid Phase, CaCrOc.
40 II. 6 10. 4 1.34 o 4.5 4.3 0.52
Solid Phase, CaCr04^30. 18 2.32 2.27 O.27 ■
o 13.0 II. 5 1.50 31 2.92 1.89 0.22
18 10.6 9.6 1.22 50 1. 12 I. II 0.13
25 100 9.1 1. 15 60 0.83 0.82 O.II
40 8.5 7.8 0.98 70 0.80 0.79 0.09
60 6.1 5.7 0.70 100 0.42 0.42 0.05
75 4.8 4.6 0.56
100 3.2 3.1 037
Densities of the saturated solutions of the above several hydrates
at 18^ are: a CaCr04.2H,0, 1.149; i3 CaCr04.2HaO, 1.105; CaCr04.HA
1.096; CaCr04.iH,0, 1.044; CaCr04, 1*023.
100 cc. 29% alcohol dissolve 1.206 grams CaCr04.
100 cc. 53% alcohol dissolve 0.88 gram CaCr04.
(F^esenius — Z. anal. Chem. 10^ 67s, 'pi^
CALCIUM CINNAMATI8
300
CALCIUl^ CnVNAMATE Ca(C«H,.CH:CHC00)i.3HA
S(H<UBILITY OF CALCIUK CINNAMATB AND ItS ISOICBRS IN SbVBRAL
Solvents.
Gma. Anhy-
Name of Salt.
FormtJa.
Solvent.
f.
drous Salt per
xooGma.
Solvent.
ciu
m Cinnainate
Ca(CACH:CHCOO)t.3HriO
Water
2
0.19(1)
u
tt
If
tt
IS
0.21^2)
a
tt
M
it
36
0.24m
a
tt
M
tt
ICO
*• 15(2)1
u
Isodnnamate
Ca(CtHfOfe)«.9H|0
tt
ao
238 (3)
tt
tt
If
Acetone
20
19.6 (3)
u
Allodnnamate
Ca(CtTiiO|)»3H,0
tt
20
2 G)
a
tt
Ca(C»HiO|)s.aH^
Water
20
10.2 (4)
tt
tt
u
Acetone
i8
2.7 (5)
u
Hydrodnnamate
Ca(C«HiO|)>?H|0
tt
14
0.19(5)
«
((
u
tt
19
0.2I(S)
tt
i<
M
Water
27
4.25(3)
tt
tt
M
Acetone
25
3-3 (3)
(x) -i De Tons, 1909; (a) - Tanigi and Cheoc&C x9oz;
1903; (5) ■■ Micnaerand Gamer, 1903.
Cs) " MirhaH, 1901; (4)." liebennann.
CALCIUM CIT&ATI Ca«(C«H«07)s.4HiO.
Solubility in Water and in Alcohol at i8^ and at 25^
(Parthefl and Httbner, 1903.)
Grams Caj(C4Hi(»MHiO per
too Gras. Solvent at:
Sdveat.
Water
Alcohol (Sp. Gr. 0.8092 = 95%)
i8*.
0.08496
0.0065
as'.
00959
D.O089
Equilibrium in thb Systeic Calcium OxiDB-CrTRic 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 trianeular diagram
and it was necessary to select the fictitious comi)Ound CcHsOr.liHiO instead of
CeHsOr 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
xoo Gms.
Sol.
Solid Phase.
Gms. per
xoo Gms. Sat.
Sol.
Solid Phase.
OHsOr.
xilbO.
CaO.
OHgOr.
ziHtfO.
CaO.
55.86
0
rtH:«07.H,0
20.3
0.3s
CiH^0K:a.4By0
54.8
0.24
ft
16.3
0.33
II
55.4
0.35
« +(aH,OT),Ca.3H,0
12. 5
039
f*
53-7
0.40
(CiH7Or)tCa.3H.0
8.3
0.28
It
48.3
0.52
M
5.2
0.25
M
42.6
0.60
tt
4.1
0.20
Quadruple pL
38.5
0.77
M
3-2
0.20
• • •
36.5
0.70
" +CiBM)TCa.4H/)
a. 4-0
0.21-0. 13
Hydrate of (CcH^)tCa*(7)
34.8.
0.77
aiU0rC:a.4H^
0.18
0.24
27.5
0.45
11
0
0.II3
Ca(OT),
CALCIUM Potaj^ium nRBOCTANIDE CaKsFe(CN)e.3HiO.
100 parts HfO dissolve 0.125 part salt at 15**, and 0.69 part at boiling-point.
(Ituiuieim and Zimmerman, 188.
100 gms. HjO dissolve 0.41 gm. CaKsFe(CN)e at 15-17^
884.)
(Brown, 1907.)
30I CALGZUM FLUORIDE
CALCIUM FLUORIDE CaFi.
One liter sat. aqueous solution contains 0.016 gm. CaFs 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 S^- ^t 25^ and 0.0167 Kin* at ao^. (Kohlimuach, 1904-05, 1908.)
Freezine-point data for mixtures of calcium fluoride and calcium iodide are
gjiven by Kuff and Plato (1903) and for mixtures of calcium fluoride and calcium
silicate by Karandeeff (1910).
CiJLCIUM FORMATE Ca(HCOO)i.
Solubility in Watbr.
(Lomaden, 1902; we also Kxasnidd, 1887.)
f.
Water.
Solution.
f.
Water.
Solution. '
0
16.15
13-90
60
17.50
14.89
20
16.60
14.22
80
17.9s
15.22
40
17 OS
14.56
100
18.40
15. S3
Gmt. CaOHiOtP
f.
Gnu.
CaCAOiP
per too GsH. Sat. SoLI
perioo
rSni*. S.t. SoL
5
40
35
4.6
60
2.7
S-2
80
1.8
s
100
0.9
Results in good agreement with the above are given by Stanley (1904).
CiJLCIUM QLTCEROPH08PHATE8 a » OH.CHi.CH(OH)CHi.OPQiCa,
^ - OH.CH,.CH.OPO,Ca.CH,OH.
Solubility of Calcium a Glycerophosfhatb in Watbk.
(Power and Tutin/ 1905; Couch, Z9X7-)
f.
O
10
20
25
Results varying from 1.7 to ^.4 gms. per 100 gms. sat. solution at or near
18^ are riven by Rogier and Fiore (1913), Willstaetter (1904) and Kins[ and
IVman (1914). It is pointed out by Couch, however, that since the solubilities
of the a and fi 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.
lOOgramsHsOdissolve i.66gramscalcium/9glyceropho6phateat20^ (Couch. 1917.)
The results of King and Pyman (1914) are: 1.4 gms. at 13° and i gm. at 15^.
CALCIUM HEPTOATI (Oenanthate) Ca[CHi(CHs)tC001t.HaO.
Solubility in Water.
(Lumaden, 1903; aee also Landau, 1893; Altsdiul, 1896.)
t . o*. so*. 40*. 6o*. So*. 'ioo*»
Gm. Ca(C7Hij08)« per
100 gms. solution 0.94 0.85 0.81 0.81 0.97 z.24
CALCIUM HYDROXIDE Ca(0H)s.
Recent determinations of the solubility of calcium hydroxide in water, ag[ree-
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 Kmopin (1914)
and Seliwanow (1914).
One liter sat. aqueous solution contains 0.305 gm. CaO at I20^ 0.169 tP^* ^^
150® and 0.084 gm. at 190''. (Herold, 1905.)
One liter of aqueous 5.2% NHs solution dissolves 0.81 gm. Ca(OH)s at about
20^ (Konowilow, 18996-;
CALCIUII HTDBOXmS
302
OALOIUM HTDROZmS Ca(OH)s.
Solubility in Water.
(Avenge curve from the results o£ Lamy, 1878; Maben, 1883-84; Herzleld, 1897* and Guthrie, j9oz.)
Grains per 100 Grams HK).
Grams per 100 Grams HiO.
» .
Ca(OH),.
CaO.
0
0.185
0.140
10
0.176
O.I33
20
0.165
O.I2S
2S
0.159
0.120
30
0.153
O.II6
40
O.I4I
0.107
fe .
' Ca(OH,).
CaO.
SO
0.128
0.097
60
O.I16
0.088
70
0.106
0.080
80
0.094
0.071
90
0.085
0.064
100
0.077
0.058
Solubility qf Calcium Hydroxide in Aqueous Solutions
Ammonium Chloride at 25°.
(Noyes and Chapin — Z. physik. Chem. a8» 500, '99.)
Mfllimols per Liter. Gnuns per Liter of Saturated Solution.
ShJoT"
OP
0.00
21.76
43 52
83.07
Solubility op
KH«a.
Ca(OH), -
CaO.
0.00
1.165
a 330
4-447
1.50
2.16
2.91
4.42
113
1.63
2.20
3-45
Ca(OH)s.
20.22
29.08
39 23
59-68
Calcium Hydroxide in Aqueous Solutions
Calcium Chloride.
of
(Zafaorsky — Z. ancrg. Chem. 3, 41, '93; Lunge — J. See. Chem. Ind. ii» 88a, 'pa.)
Grams CaO Dissolved per 100 cc. Solvent at:
Concentration
cf CaClsSolutians,Wt.%.
so"
40 .
9.I162
O.I160
O.I419
O.1781
0.2249
0.3020*
0.3680*
* Indicates cases in which a precipitate of calcium ozychloride separated and thus removed some of
the CaCh from solution.
The results in 0% CaCh solutions, «.«., in pure water, are high when compared with the average
lesuhs given above.
Solubility of Calcium Hydroxide in Aqueous Solutions of Calqum
Chloride at 25*.
(Schieinemakers and Figee, 19x1.)
Oms.perxooGms.Sat.SoL ^ ..,«. Gms. per 100 Gms. Sat. Sol.
O
S
10
IS
90
as
30
0.1374
0.1370
o . 1661
0.1993
0.1857*
O.I66I*
0.1630*
6o*.
o . 1026
o . 1020
0.1706
o . 2204
o . 2989
0.3664
8o*.
0.0845
o.o93i
0.1328
0.1736
o . 2295
0.3261
0.4122
loo".
0.0664
0.0906
0.1389
o . 1842
0.2325
0.3710
0.4922
iCaCls.
5.02
10
15 14
18.15
18.01
21.02
28.37
32.67
CaO.
O.IOX
O.II5
0.140
0.148
0.152
0.147
0.170
0.225
Solid Phase.
Ca(0H),
i<
II
" +CaClt.4Ca0.X4H,0
Caa2.4Ca0.i4H«0
11
ff
CaCla.
33-21
33 72
34.36
3861
41.32
44.30
44.61
44.77
. Solid Phase.
CaO.
0 . 245 CaCli.4CaO.X4HjO
0.254 " +CaCIi.Ca0.aHiO
0.173 CaCIi.CaO.aHt0
0.060
0.048
0.030
0.029
<i
«
If
" +CaClt.6HB0
CaCIi.6Hs0
48®, and 50® are given by
Ca(OH),?
Data for the above system at 10", 25®, 40', 45
Milikau (1916).
Data for the solubility of calcium hydronde in aqueous calcium iodide solu-
tions at 25^ are also given by Milikau.
203
CALCIUM HTDROZmS
Solubility of Calcium Hydroxidb in Aqueous Solutions of Calcium
Nitrate at 25® and at 100**.
(BasBctt and Taylor, 1914; see also CameroD and Robinson, 1907a.)
Results at 25"".
Results at 100®.
Results at 100'' (Con.)*
Gma. per 100 Gms.
Gms. per :
100 Gms.
Gms. per
TOO Gms.
£t.
Sol. Solid Phase.
Sol.
Solid Phase.
1 <
. Sol. Solid Phase.
'CaO.
CaCNOD^
CaO.
Ca(NOi),.
CaO.
Ca(NO,),.
0.1x50
0 Ca(0H)s
0.0561
0 Ca(0H)s
1.576
58.67 CaiNi0r.9Hi0
0.0978
4.836
0.0550
2.42
t(
1.348
60.44 "
0.1074
9.36
0.0624
4.91
(«
1. 167
62.82 «
O.II93
13.77
O.IIIO
15. 39
M
1.077
66.44 "
0.1444
22.46
0.1200
16.10
M
1.X4X
69.12 "
0.1650
27.83
0.155
21.86
U
" +avery
O.1931
32.94
0.269
33 03
U
1.252
70.60 little Car
0.2579
40.66
0.480
42.26
it
•
NsOr.iH^
0.3060
44.44
0.973
50.94
U
1.203
70.40 OuNsOi.iHflO
0.2802
45.28 CaaNs0r.3H«0
1. 261
53.75
a
1. 103
71.44
0.23x4
47.79
1-477
5540
w
0.937
73.85
0.1894
51.07
1.476
55-43
M
0.849
75-74
0.1659
53 • 20
1. 491
55-65
(t
0.815
76.94
0.1486
55 • 25
1.635
56.89!
1" +CaiN«0r.
\ aH«0
-0.804
77.62 Ca(NO^t
0.0836
57 . 72 Ca(N0k)MH«0 1 .686
57-03!
0.412
77.74
0
57.98
1.596
57.91
CaaN^.aH/)
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, 2906.)
Gma. per zoo cc. :>at. boL
Solid
Phase.
ums. per too cc. ^t. bol.
Solid
CaSOt.
CaO. '
CaSOt.
CaO.
Phase.
0
O.II66
Ca(OH)s
0.1634
0.0939
CaS0i.aB^
0.0391
O.II4I
ft
0.1722
O.061I
M .»
0.0666
0.1150
ti
0.1853
0.0349
«
0.09SS
O.I215
It
•
O.I918
0.0176
M
O.I2I4
0.1242
u
0.2030
0.0062
«
0.1588
0.1222
ft
+CaS0i.2Hi0
0.2126
0
«
The mixtures were constantly agitated at 25^ for two weeks.
Solubility of Calcium Hydroxide in Aqueous Solutions of Potassium
Chloride and of Sodium Chloride.
(Cabot, 1897.)
In KCl Solutions.
In NaCl Solutions.
Gms. of the
Chloride
per Liter. .
Gnis.<
CaO per Liter at:
Gms.
, CaO per Liter at:
' 0-.
IS*.
99*.
o*.
IS*.
99*.
0
30
60
120
1.36
1. 701
^•725'
1. 718
I-3I
1.658
1.674
1.606
0.63s
0.788
0.876
0.894
,1.36
1. 813
• ■ •
1.86
I-3I
1.703
1.824
1.722
0.63s
0.969
1.004
1.015
240
1.248
1. 199
0.617
1-37
1.274
0.771
320
• • •
• • •
• • •
1.054
0.929
0.583
Results in harmony with the above for the solubility of calcium hydroxide
in aoueous solutions of potassium chloride at 50^, are given by Kemot, d'Agostino
and Pellegrino (1908). .
CALCIUM H7DB0XIDS
304
Solubility of Limb in Aqueous Solutions of Sodium Chloridb alonb and
CONTAINING SODIUM HtDSOZIDB.
CliaiCRt. 1905.)
_ ^ Q G«i. CaO per Lker of SofatioH.
O
5
10
as
so
7S
100
NaOH.
1-3
1.4
1.6
1-7
1.3
1.9
1.85
08
0.9
i.o
I.I
1-4
1.4
per Liter.
0.33
o-SS
G. NaQ.
per Liter.
ISO
^75
183
335
350
300
• • •
Gms. CaO per liter of SolutJon.
o^J^aOH 4^09-NaOH
Without
NaOH.
I
I
I
I
I
I
6S
6
6
4
3
I
per Liter.
I -as
1.3
1.3
1.0
0.9
0.7
per Liter.
0.44
0.33
Solubility of Calcium Hydroxidb in Aqubous Solutions ob
Sodium Hydroxide.
(d'Anielme — Boll. see. diim. [3] a(W 9381 '03.)
ConoentratioD of NaOH:
N«raudatr.
Gms. per Liter
0
0
N/ioo
0.4
N/2S
1.6
N/15
3.66
N/8
S-oo
N/S
8.00
N/2
30. CO
Liter Sat. Soluticn at:
30 .
SO*.
7o».
lOO*.
1. 170
0.880
0.7s
O.S4
0.94
0.65
O.S3
0.3s
O.S7
0-3S
0.325
0.14
0.39
0.30
O.II
0.0s
0.18
0.06
0.04
O.OI
O.II
0.02
001
trace
0.03
trace
0.00
0.00
For results upon mixtures of calcium hydroxide and alkali carbonates
and hydroxides, see Bodlander — Z. angew. Chem. 18, 1x38, '05.
Solubility of .Calcium Hydroxide in Aqueous Solutions or
Glycerol at 35^
(Hen andKnoch— Z. anors. Chem. 46, 1931 '05; for older determinationa, see Berthdot— >AiiB.cftim
P^y** [3] 4^ Z76; and CarlM — Arch. Pharm. [3] 4, 558, '74.)
Gms. per xoo oc. Solutioa.
Density of
Solutions
Glycerine
In Solution.
MOHmob
iC»(qH),wr
1.0003
0.0
4.3
1.0244
7IS
8.13
I -0537
20.44
14.9
1.0842
31 ss
22.5
I "37
40.9s
40.1
I 1356
48.7
44.0
1.2073
69.2
9S-8
Ca(OH),
- CaO.
O.IS93
0.1206
0.3013
0.2281
0.5522
0.4180
0.8339
0.6313
1.486
I 135
1. 631
1.234
3SSO
3.687
Dat& tor the solubility of calcium hydroxide in aqueous solutioiis of phenol
at 35** are given by van Meurs (1916).
305 CALCIUM HTDBOXIDX
SoLUBiLiTT or Calouii Hydbozidb IK Aqubous Solutions op Glycbiol
AND OT.CaNB SvGAR AT 25^
(CunenMi and Fatten. 191 1.)
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.
^of Gms. per 100 Gms. Sat. SoL Solid ^of Gms. per too Gms. Sat. Sol. SoUd
Sat. SoL Ca(OH)i. OBWOEDr !*>»«. Sat.So|. Ca(OH)t. OsH^Ou ?»>"••
0.983 O.I17 O CaiOBk I 0.188 0.62 Ci(QH>i + Si«M
1.008 0.178 3.50 * 1.021 0.730 4.82 ••
... 0.413 15.59 - 1.037 I. 355 7.50
1.042 0.48 17.84 ** 1.067 3.21 XI. 90 "
1.088 0.88 34.32 " 1. 109 5.38 17.42 •
1. 149 1.34 55.04 " 1. 123 6.07 19.86
Sglubilitt of Calcium Htdrozidb in AguBoys Solutions of Canb Suoar
AT 80*.
(von Ginneken, 191 1.)
Gms. per too Gms. Sat. Sol. Solid Gms. per 100 Gms. Sat. Sol. Solid
' CaO * S^. ' !*»>"«• ' So * Su9[r! ' ^^»^
O.II7 4.90 Ca(OH)i 0.358 19.50 Ca(OH)t
0.189 9.90 " 0.548 24.60 "
0.230 14-75 " 1.017 29.70 ••
Solubility op Limb in Aqubous Solutions of Sugar.
(Weisbeii— Bull. soc. cUm. [3] ai» 775t '99O
The original results were plotted on cross-section paper and the
following table constructed from the curves.
i8t series, t^ «>
i6'-i7^
2dp series t° >
-iS^
§^
100 Gms.
idoo.
G. CaO per 100
Gms. per xoo Gms.
SoIuHmi.
0. CtO per lee
Sugar.
CaO.
Gms. Sugar in Sol.
Sugar.
CaO!
Gmi. Sour in Soi«
I
0.30
3SO
I
0.50
62.5
a
0.56
28.7
a
0.7s
3<5o
3
0.85
28.0
3
1.02
3' 5
4
1. 12
27.7
4
1.22
30.9
S
1.40
27 S
5
1-45
28.5
6
1.65
275
6
1.67
27.7
8
2.22
27-5
8
2.22
37 s
10
2.77
27 S
10
2.77
27 S
12
3-27
27-5
12
3 27
27 S
14
3.85
«7S
14
385
27 S
In the second series a verv much larger excess of lime was used than
in the first series. The autnor gives results in a subsequent paper, —
Bull. soc. chim. [3] 23, 740, '00, — which show that the solubility is also
affected by the condition of the calcium compoimd used, i.e., whether
the oxide, hydrate, or milk o£ lime is added to the sugar solutions.
A very exhaustive investieation of the factoni which influence the solubility
of lime in sugar solutions is aescribed by Claasen (1911).
OALGXDM lODATB 206
OAUnrM lODATS Ca(IO0t.6H.O.
Solubility in Watbr.
Qiilbm lad FaolcBcr. 90^ iJUt '97; W. Abh. p. t. BddniHtak a, 448. '00.)
GlDS.
Mdt.
Cms.
Mob.
* «
oao^
Ca(IOi)>
Solid
^. CaaOk)*
CaaOfe)t Solid
• •
per loe
Gma. Sol.
per 100
Phaie.
* per 100
Gins.Sol.
per 100 Phue.
0
o.io
0.0044
Ca(IO,) .6H,0
21 0.37
0016 Ca(IO,),.H,0
10
017
0.007s
((
35 048
0.021 "
18
025
O.OII
u
40 0.52
0 023 "
30
04^
0019
*t
45 0.54
0.024 "
40
0.61
0.027
u
50 0.59
0.026 "
so
0.89
0.040
*t
60 065
0.029 "
54
1.04
0046
It
80 0.79
0034 "
60
I 36
0.063
11
100 0.94
0.042 **
r
)ensitv (
Df solutioi
a saturated
at ]
[8^« i.oo.
OALOIUM lODIDB Cal,.
Solubility in Water.
(Avente cum from the Rsoltfl of Kremen — PoKK. Ann. 103, 65, '58; Etaxd — Ann.diim. pliyft.(7]
a* 53>* '94)
t;
Cms. Call per xoo
Gma. Solution.
f.
Gms. Calf per xoo
Gnu. SoiutiaD.
« e Gms. Cala p
* * Gms-Sdol
0
64.6
30
69
80 78
10
66.0
40
70.8
ZOO 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).
CILCIUM lODO MEBCUaATI.
A saturated solution of Cali and Hgis in water at I5*9^ was found by Duboin
(1906) to have the composition CaIs.i.3HgIs.i2.3HsO; d » 2.89 and the solid
phase in contact with the solution was CaIs.HgIi.8HsO.
CALCIUM PerlODIDE CaU
Data for the formation of calcium periodide in aqueous solution at 25^ are
given by Herz and Bulla (191 1). (See reference note under calciimi perbromide,
p. 189.)
CiJLCIUM LACTATI Ca(C«HioO«).5HsO.
100 gms. HiO dissolve 3.1 gms. of the salt at o^ 5.4 gms. at 15^ and 7.9 gms.
at 30^. (Hill and Coddns, i9xa.)
CALCIUM MALATI CaC4H40«.HsO.
S(h.ubility OF Calcium Malatb in Water and in Alcohol.
(PartbeQ and Httbner, 1903.)
100 gms. HiO dissolve 0.9214 gm. CaC4H40i.HsO at i8% and 0.8552 gm. at
25".
100 gms. 95% alcohol dissolve 0.0049 gm. CaC4H40i.HiO at 18"*, and 0.00586
gm. at 25*.
207
CALCIUM HALATB
CALCIUM (Neutral) BCALATE Ca(C4H40t).3HsO.
CALCIUM (Acid) MALATE Ca(C4H«0«),.6HsO.
CALCIUM MAI.ONATq:Ca(CaisO«).4HsO.
Solubility of Each in Water.
(Iwig aa^Hecht, x886; Cantoni and Basadonna, 1906; the malooate, WcKynaki^ 1886.)
(
Ca. Neuti
ral Malate.
Ca. Acid Malate.
Ca. Malonate.
Gms. Ca(C«HfOi)
per 100
Gina.'Ca(C4HiOk)tper
r.
Gnu.
Gmn.
cc. SoL
100
Gms.
Gms. Ca(CiHA)i)
per 100 Gms. HiO.
HiO.
SoL
(C and B).
^ater.
Solution.
0
• • «
• • ■
• • a
• • •
• ■ •
0.290^0.374)
0.330 (0.419)
10
0.85
0.84
• • •
1.8
1.77
20
0.82
o.8x
0.907
1-5 •
1.48
0.365 (0.460)
30
0.78
0.77
0.83s
2
Z.96
0.396 (0.49SJ
40
0.74
0.73
0.816
5-2
4.94
0.422 (0.524)
so
0.66
0.6s
0.809
IS- '
13 09
0.443 (0.544)
57
O.S7
0.56
• « •
32.24
24.29
■ • •
60
0.58
0.58
0.804
26
20.64
0.460
70
0.63
0.63
0-79S
ZI
9.91
0.472
80
0.71
0.70
0.7S4
6.8
6.37
0.479
90
• • •
• • •
0.740
The results for calcium malonate eiven 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(N0t)s.4H,0.
Solubility in Water.
(Baaaett 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(NOi)f SoUd 4.
per 100 Gms. Phase.
Sat. SoL
53 • 55 CaCNOdMHsO 45
f.
Gms.
Ca(NO«)fl
per xoo Gms.
Sat. SoL
Solid
Phase.
f.
Solid
Phase.
- 0.4
1.4
Ice
10
- X.4
4.78
M
15
- 1.9
6.53
M
20
- 305
10
«f
25
- 4.15
12.98
M
30
-15.7
3313
it
35
— 21.7
38. J
• • •
U
40
— 28.7
42.4
— 26.7
43-37 CaCNOdMHW) 42.4
— 10
47.31
it
42.7
0
50.50
tf
42.45
5
51.97
U
40
tm.pt.
54.94
56.39
57 98
60.41
62.88
66.21
68.68
68.74
...t
71.7
«(
M
M
CI
If
«
l(
«f
«
50
51
51. I
49
51
55
80
100
125
147-5
Gms.
Ca(NO0t
per xoo Gms.
Sat. Sol.
71.45 Ca(NO0i.3BiriO
73 . 79
74.73
77.49 CaCNOk)s.aH«0
78.05
ft
(f
it
70.37 Ca(NQ0t.3HiiO 151
* Eutectic
78.16
78.2
78.43
78.57
78.8
79
Ca(NOi)s
u
M
M
l<
Solubility of thb Unstablb Calcium Nitratb Tbtrahydratb fi in Watbr.
(Results supplementary to the above.)
CTaylor and Henderson, 19x5.)
Gms. Ca(N0k)i
f.
per 100 Gms.
Sat. Sol.
Solid Phase.
f.
0
50.17
aCa(N0a)t.4H«0
38
32.2
56.88
f(
39 ,
25
57.90
If
39.6 (m. pt.)
30
60.16
f«
39 (reflex pt.)
30
61.57
^Ca(N0di^B«0
40
34
63.66
((
42 . 7 rm. pt.)
42.4 (reflex pt.)
35
62.88
aCa(N0a)i.4HK)
38
64.34
M
25
Gnu. C
aCNOJ
i
per 100 Gms.
Solid Phase.
Sat.
SoL
66.
65
^CaCNC^MHsO
67.
93
i<
69
SO
u
7534
u
66
22
aCaCNOi)MH«0
69
SO
u
71
.70
M
77.30
Ca(NOds
CALCIUM NTTRATI
308
S(M.uBiLiTY OP Calcium Nitrate in Aqueous Solutions of CALouif
Thiosulfate at 9* and at 25" AND Vice Versa.
(Kremann and Rodemond, 19x4.)
Results at 9^
Results at
25*.
Gms. per too
Gms. Sat. SoL
Solid Phase.
Gms. per xoo
»Gms.Sat.Sol.
Solid Phase.
Ca(NOk)i.
CaSiOs.
Ca(N0i)i.
CaSiQi.
46.02
5-46
Ca(N0|)MH:0
54.03
4.27
Ca(N0i)MHi0
45.68
6.81
" +CaSi0^6H^
SO. 25
9.10
M
27.92
10.46
<W^^H/^
45.92
13
'* +CaS^61b0
10.49
22.81
«
42.93
13.83
CaSiQi.6HiO
• • •
2933
If
32.01
17.09
M
19.51
23.78
M
8.15
29.85
M
Solubility of Caluum Nitrate in Aqueous Solutions
OF Sodium
Nitrate at 9** and at
25* AND Vice Versa.
(Kiemann and Rodemund, X9X4-)
Results at
9°.
Results at 25
0
•
Gms. per loc
> Gms. Sat. Sol.
CnlM PhAWk
Gms. per xoo Gms. Sat. SoL
Solid Phase.
daCNQOi.
NaNOi."
ouiia A nase*
•Ca(N0i)i.
NaNOi.
47 SI
951
CaCN0^i.4lb0
54.58
7.25
Ca(N0«>MHi0
46.08
12.56
" +NaN0*
53-22
10.70
M
26.67
23.32
NaNOi
52.73
i2-.o8
•'+NaNOi
11.76
34.26
u
52.40
11.88
NaNOi
37 31
19.48
ft
26.91
24.98
f«
14.61
36.12
•f
These authors also give the complete solubility relations of the reciprocal
salt pairs, Ca(NOi)i + NasSsOi t? 2hfaN0» + CaSsOs at 9** and 25**.
Solubility of Calcium Nitrate in Aqueous Solutions of Nitric Acid at 25*.
(Bassett and Taylor, X9X2.)
(The mixtures were shaken intermittently, by hand, during quite long periods;
one week was allowed between duplicate determinations.)
Gms. per loo Gms. Gms. per loo Gms. Gms. per xoo Gms.
Sat.
Sol.
Solid Phase.
Ca(NOI)«.
HNQi.
57.98
0 <
ZaQfOth-ABd
54.82
3.33
u
52.96
587
51.58
7.21
47.82
XI. 27
45. 59
13.71
40.70
19.65
38.17
22.80
34.46
28.81
•"
a
Sol.
Solid Phase.
t. Sol.
Solid Phase.
Ca(N0dt
Ca(NOi)t. HNOi. Ca(NOi)t. HNOi.
CaCNQ0s.4HiO 32.84 32.63 Ca(NQ0t.4H^ 934 65.69 Ca(Nai)i.2£bO
32-50 33.52 " 8.52 67.20
33.44 35.63 Ca(N0i)i.3Hi0 5.06 71. 12
29.05 41.66 " 2.53 74.77
2779 45.70 " 1.05 78.56
31.09 40.56 Ca(NO0t.aH«O 0.54 80.83
26.07 45.70 " 0.36 85.83
17.41 55.48 " o.ox 90.90
12.25 62.05 " o 96.86
Freezing-point data for the Ternary System Ca(NOi)i-|-KNOi + NaNOt are
given by Menzies and Dutt, 191 1.
Solubility of Calcium Nitrate in Several Organic Solvents.
«
w
<f
l(
u
Solvent.
f.
^ Gms. Ca(N0i)9 per xoo Gms
^ Sat. Solution.
Authority.
Methyl Alcohol
25
65.5
(D'Ans and Siesler, 1913.)
Propyl
25
S^'S
it u
i Butyl "
25
25
M M
Amyl
25
13.3
M M
Acetone
25
58.5
li M
Methyl Acetate
18
41 (i8at.i6L-]
[.313)
(Nwimaim, 1909.) J
209
CALCIUM NITRATE
SqLUBIUTT of CALaUK NiTRATB IN AqUEOUS SOLUTIONS OF EtHYL AlCOHOL
AT 25*. (D'Aas uid Siegler, 1913)
Gms. prr too Cms. Sat. Sol. _ ... ... Gms. per xoc
> Gna. Sat. Sol.
SoUdPhaK.
CtHrf)H
Ca(NCW<.
CtHiOH.
Ca(NO>)i. '
0
S7-5
Ct(NQ0«.4H/)
IS-2
69.52
Ct(NO0< oiHtabk
8.1
SS-2
It
20.4
66.08
M If
14.1
52-9
«
35-9
57-7
If fl
22.3
50.2
w
41.8
51 -4
ff ft
29.4
49
<(
27 -39
61.96 Ct(N04tiUUe
31.2
52
II
28.5
61.15
V
29s
56.2
11
29.6
60.3 •
" +Ca(N0^s.ar*HiOH
27.8
60
M
60.2
38.6
Ca(N0^s.aCiHiOH
26.5
62.3
" +Ca(N0d«
54.6
41.9
*i
0
82.5
Ca(NOi)s ttuUble
42.5
50-97
■•
5-8
77
<i (1
35-8
55-3
M
GALCIDM NITBm Ca(N0i),.4H,0
•
Solubility in Water. (Osw»w. 19x4.)
f.
^cSf^dSr soHd nu.
*•.
^G^IS'^ solid Ph.«.
- 4
16.7
loe
18.
5 43
CaCNOOMH«0
- 9-3
2SS
i«
42
51.8
If
-12.5
295
II
44
53-5
" +C«(NO0i.aHiO
-145
32
II
54
55-2
Ca(NO0i.3HflO
-17s
35
" +Ca(NO0MlW) 64
58.4
II
- 9-S
36.2
Ca(NOOMH«0
70
60.3
II
0
38.3
II
73
61.5
11
16
42.3 (*
• -1.4«>S) "
91
71.2
«j
An aqueous solution simultaneously saturated with calcium nitrite and silver
nitrite, contains 92.4 gms. Ca(NOt)s + ii-2 gms. AgNOs per 100 gms. HtO at 14^
(Oswald. 1914.)
100 cc. sat. solution of calcium nitrite in 90 % alcoholcontain 39 gms. Ca(NOs)s.
HjOat20^
100 cc. sat. solution of calcium nitrite in absolute alcohol contain i.i gms.
Ca(NOt)j.H,0 at 20**. (Vogd, 1903.)
CALCIUM OLIATI (Ci»H»0,)Ca.
One liter water dissolves about o. i gm. calcium oleate at t^not stated. (Fahrion, 19x6.)
100 gms. glycerol (old^i.i 14) dissolve 1.18 gms. calciumoleate at t° not stated.
(Amflin, 1873.)
CALCIUM OXALATE Ca(COO)s.HA ^.■
Solubility in Water, by Electrolytic Conductivity Method.
(HoUeman, Kohliauach, and Row, 1893; Richazds, McCafErey, and Bisbee, 1901.)
*o
Gms. CaCi04 per
Liter of Solution.
t^
Gms. CaCsOi per
» .
•
Liter of Sdudon.
13
0.0067 (H)
^s
0.0068 (R, McCandB)
ta
0.0056 (K and R)
50
0.009s "
24
0.0080 (H)
95
0.0140 "
ilubd
LITY OP CALaUM OXALATE IN AqUEOUS SOLUTIONS OF ACETIC Ac
26°-^7''. (Herz and Muhs. 1903.)
Normality of
G.CHiCOOH
Residue from 50^051
.Aoetic Add.
per xoo cc. S6L.
cc. Solution.
0
0.00
0.0017
0.58
3'^
0.0048
2.89
17 -34
0.0058
S-79
34-74
0.0064
The residues were dried at 70^ C.
CALCIUM OXALATE 2x0
SOLUBQ^ITY OF CaLCIUK OXALATE IN AqUBOUS S(X.UTI0NS OF. HYDROCHLORIC
Acm
AT
25*.
(Hendenon and Taylor, 1916.)
•
NomuHty of HCL
Cms. CaCA per
liter Sat. Sol.
Nonnality of HQ.
Cms. CaOOi per
Liter Sat. Sol.
0
0.009
0.500
2.638
0.125
0.717
0.625
3 319
0.250
1-359
0.750
3922
0.37s
2.019
I
5 -210
These authors also give data showing the effect of increasing amounts of KCl
and KNOi upon the solubility of calcium oxalate in o.^ normsu HCl at 25^, and
also of the effect of increasing amounts of potassium tnchloracetic acid upon the
solubility in 0.5 normal trichloracetic acid, and of increasing amounts ot potas-
sium monochloracetic acid upon the solubility of calcium oxalate in 0.5 normal
monochloracetic acid.
Solubility of Calciuk Oxalate in Aqueous Solutions of Sodium Chloride
.AND OF Sodium Phosphate.
(Gerard, 1901.)
Salt in Aq. Gnu. Salt ^ Gms. CaC«Oi Salt in Aq.
Sdution. per Liter^ * per Liter. Solution.
NaCl I 25 0.0075 NaCl
" 5 25 0.0188 NaaHCPGOi
" 10 25 0.0255 "
<c
Gms. Salt
per Liter.
f.
Gms. CaOOi
per Liter.
25
4.8
37
IS
0.0414
0.016
4.8
37
0.033
25 25 0.0291
One liter 45% ethyl alcohol dissolves 0.000^25 gm. calcium oxalate, temp, not
stated. (Gueiin, 1913.)
CALCIUM OXIDE CaO.
100 gms. molten CaCls dissolve 16.2 gm. CaO at about 910^
(Amdt and Loewenstetn, 1909.)
Data for the systems, CaO + MgO and for CaO + AltOi -f MgO are given by
Rankin and Merwin (1916); for CaO -f AliOi -f SiOi by Rankin and Wright
(191 5); for CaO + Fe»0» by Sosman and Merwin (1916); and for CaO + MgO
-f SiOj by Bowen (1914).
Data for the system CaO + C + Cad + CO are given by Thompson (1910).
CALCIUM PHOSPHATE (Tribasic) Ca«(P04)s.
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
mav 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 CasCPOt)! the amount whicn is dissolved
by COs free water at the ordinary temperature, as calculated from the calcium
determination, is 0.0 1 to o.io gram per liter, depending upon the conditions of
the experiment. Water saturated with COs 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,, 27f 1512, 1905.
axx
CALCIUM PH08PHATB
OALOIUM PH08PHATK (Dibasic) CaHPO^.aHA
Solubility in Water.
(Cameroo aod SddeO — J. Am. Chtm. Soc. 26, 1460* 'o^^; see also Rindell — Compt. rend. 1349 iia» '00;
Magnanini — Guz. chim. ital. 3X« II, 544, '01.)
I liter of CO, free water dissolves 0.136 gram CaHP04 at 25®.
I liter of water sat. with CO, dissolves 0.561 gram CaHP04 at 25**.
Solubility op Di Calcium Phosphatb and op Mono Calcium Phos-
phate IN Aqueous Solutions op Phosphoric Acid at 25**.
(Cunercn axid Seidell — J. Am. Chem. Soc. a7» x5o8» '05; Causae — Compt. remi. 1x4, 414, 'pa.)
PsOfl per liter
in Excess of
that oomfained
withCa.
Grains per liter of
Sohitiaa.
Gms. i>er liter
Calc fmm r*aO V/wnwI.
'CaO.
PaO«.
\.AH*. MA\^M
1.71
4.69
4.15
CaHPO,
"57
3^H
28.05
It
23-31
75 -95
56 -53
it
39.81
139.6
97.01
€t
49.76
191 .0
120.7
ts
59 40
334.6
144. 1
Si
70.31
279.7
170.6
it
77.00
317.0
174.2
(321-3
CaHPO. or
CaH,(P6,),
72.30
351-9
301.6
CaH,(PO^,
^33
361. 1
289.3
((
5998
419-7
250.2
a
53 59
451-7
223.7
a
44.52
505-8
185.8
a
39 89
5383
166.4
it
Solid Phase.
2.53
21.5
46.45
89.0
128.0
159-4
190.7
226.0
122.2
169.0
186. 1
267.9
316. 1
393-1
437-4
CaHP0^.2H,0
tt
it
a
a
a
a
CaHP0..2lL0+
CaH,(PO ),.ILO
CaH,(PO,),.H,0
it
a
ii
a
a
Density of the solution in contact with both salts at 25^ « 1.29.
Solubility
Results at 25
OF Calcium Phosphates in Aqueous Solutions of Phosphoric
Acid at Different Temperatures.
(Bassett, Jr., 1908, X9X7.)
Results at 40^ Results at 50.7^.
Gms. Der xoo
Gms. Sat. Sol.
Solid Phase.
Gms. per xoo
Gms. Sat. Sol.
SoUd Phase.
Gms. per xoo
Gms. Sat. Sol.
Solid Phase.
CaO.
P^Oi.
CaO.
P«Oi.
' CaO.
PiO^
3.088
36. IX CaHiP«0t.Hi0
1.768
42.42
CaH«PhOs.H|0
0.336
62.01 (
CmEaP^+
4.908
28.34 "
3.584
36.79
«
CaHiPsOt-HiO
S.809
24.20 « +CaHP0i
S.755
27.25
" +CaHPOi
0.635
58.08 (
CaHJ>K)s.HiO
5.523
22.90 CaHPOi
4.813
21.67
CaHPOi
1.428
50.25
<<
4.499
17.55 "
3.810
16.3s
(f
2.974
41.92
If
2.638
9.100 "
2.536
9.905
(1
4.880
33.18
»i
1.878
6.049 "
1.847
6.979
u
5.725
29.61
" +CaHPOi
0.826
2.387 "
1.267
4.397
M
3.507
15.48
CaUPOi
0.165
0.417 ( " CaHPOi.
0.166 ( aHtO
0.576
X.819
«
2.328
9.465
f(
0.07
0.156
0.426
<f
1.563
6.157
tt
0.06
0.140
0.0592
0.158
11
0.692
2.281
tt
■
0.05
0.1 18
0.0508
0.128
CasP<Ot.HiO
0.0596
0.1527
CaHPOi.aB^
0.04
0.093
0.0098
0.0262
<•
0.0514
0.1331
CasPsOs.HiO
0.03
0.070
Morebaiirth»iP°-^?°^
trace
CaiPflOi^HflO
0-0351
0.0942
fi
0.02
0.047
CaHPOcaHiO
0.0814
«
14
0.0106
0.0309
M
0.01
0.023
0.0840
tt
C4
O.OCO7
0.0007
tt
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 ne3ct page.)
OALGZUM PH08PHATI8
212
S(M.uBn.iTY OF Calcium Phosphates in Aqueous Solutions of Phosphosic
Acid at Temperatures above ioo^.
(Baaaett, Jr., 1908.)
Gms. per xoo Cms Sat. Sol.
r.
100
11$ b. pt.
132
169
CaO.
2.503
5-623
4327
4.489
PiO.
53.71
43.60
53.43
63.95
Solid Phase.
CaH<P,0i+CaHiP^Hd0
CaHiP|Ot.Ha0+CaHPOi
CaH<P«0t+CaHiP|0i.Hfl0
CaHiPA
The quintuple points for the system determined by dilatometer experiments
are as follows:
152
21
36
5.60
5.81
0.05x4
53 CaHiPtOi+CaH<PAH|0+CaHFOc
23 . 5 CaHiP«0i.Hy0+CaHP0i+CaHP0i.2H,0
0 . 14 CaHF0i+CaHP0i.2H<0+CasP,0i.H]0
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 Camefion
and Bell (1906).
One liter of ac^ueous 0.005 ^ potassium bitartrate solution sat. with calcium
phosphate, contams 0.08 gm. Ca and 0.181 gm. H«P04 at 25**. (Magnanini, 1901.)
Solubility of Calcium Phosphate in Aqueous Salt Solutions Under 2
Atmospheres Pressure of COi at 14®.
(Ehlert and Hempd, 1912.)
Gms.
Caa(PO«)t
per Liter
Solveat.
0.238
Sak in Aq. Solvoit.
Gms. Salt
per 100
Gms.Hi0.
Water
u
(NH«)sS04
((
Mga«.6H«0
MgS04.7HiO
((
MgCls.KCl.6HsO
It
45-74
1. 371
cone.
X.293
565
2.413
cone.
5.885
86.9
1.387
cone
a. 892
105.3
1.9738
cone.
3.6001
79.2
1.577
cone.
1 .154
Salt in
Aq. Solution.
•
Gms. Salt
per 100
Gms. HsO.
Gms.
Ca«(PO0«
per Liter
Solvent.
MgSO4.KsSO4.MgCls.6HtO
70.95
1.777
fi
cone.
2.49X
KsS04
74.5
4.904
((
cone.
4.765
NaQ
50
1. 321
((
cone.
0.64X
NaNOk
72.7
Cone.
1.583
u
0.864
NasS04.ioH*0
137.7
2.491
u
cone.
3.227
Data for the solubility of calcium phosphate in aqueous saturated solutions of
carbon dioxide containing ammonia are given by Foster and Neville, 19 10.
CiJLCroM PILABOONATI (Nonate) Ca[CH,(CH,)7 C00]i.H,0.
CALCIUM PROPIONATE Ca(CH,.CHiCOO)i.HsO.
Solubility of Each in Water.
(Lumsden, 190a; Knsnicki, 1887.)
Calcium Pelaigonate.
Calcium Propionate.
Gms.
Gms. CaCCHi.CHfCOOt per xoo Gms.
t»
Ca(CHi(CHs)7C00]i
per zoo Gms. HiO.
V •
Water.
Solution.
0
0.16
42.80
29.97
20
0.14
39 -85
28.48
40
013
38.4s
27.76
60
0.12
38-25
27.67
80
o.iS
39 85
28.48
90
0.18
42.15
29.66
100
0.26
48.44
32.63
213 CALCIUM 8ALICYLATB
CILCIUM 8AUCTLATI Ca(C«H4.0HCOO)t.3HsO.
100 grams of the saturated aqueous solution contain 2.29 grams of the an-
hydrous salt at 15^ find 35.75 grams at I00^ (Tarugi and Checdu. Z901.)
OALOIUM SKLBNATE CaSeO^.
Solubility in Water
(Eurd — Ann. chim. phyt. [7] 2, S3»t 'mO
t*. -X*. +5'. »©•. si*. 67*.
6ms. per ICO gms. soL 7.4 7.3 7.6 6.8 5.1
The accucacy of these results appears questionable.
OALOIUM 8ILI0ATE CaSiO,.
Solubility in Water and in Aqueous Sugar Solutions at 17*.
(Wdsberg — Bull. soc. chim. [3] 15, X097, '96O
The sample of calcium silicate was air dried.
Grama per xoo cc. Saturated Solution.
Solvent. At X7*. After Boiling and Ffltering Etot.
CaO(det.) CaSiO|(calc.) CaO(det.) CaSiOt(calc.)
Water 0.0046 0.0095
10% sugar soL 0.0065 0.0135 00094 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.
CaSiO|-fCaS (Lebedew, xgxx.)
" + CaTiOi (SmolenslEy, xgxx-xa.)
" -f LiiSiOi (Wallace, 1909.)
** + MgSiOs (Allen and White, xQxx; Ginsbeig, 1906.)
" -|- MnSiOi (Ginsberg, 1908, 1909.)
" + NasSiOs (Wallace, 1909; KultaachefiF, 1903.)
CALCIUM 8UCCINATI Ca(CsHiO,)s.
CALCIUM (Iso) SUCCINATE CaCHi.CHCs04.H,0.
Solubility of Each in Water.
(Miosynski, 1886.)
Calcium Succinate. Calcium Iso Succinate.'
f.
Gma.
Ca(CHi0^t
per xoo Gms.
HiO.
f.
Gms.
Ca(C«HfO0«
per xoo Gms.
HiO.
V.
Gms.
CaCCsHiOOs
per xoo Gms.
HaO.
f.
Gms.
Ca(CsHA)t
per xoo Gms.
HiO.
0
1. 127
SO
1.029
0
0.522
SO
0.440
10
1.220
60
0.894
10
0.524
60
0.396
20
1.276
70
0.770
20
0.517
70
0.342
40
1. 177
80
0.657
40
0.47s
80
0.279
100 cc. HsO dissolve 1.424 gms. CaC4H404.HsO at 18"* and 1.436 gms. at 25"*
(Partheil and Httbner, X903.)
100 gms. HtO dissolve 1.28 gms. CaC4H404 at 15^ and 0.66 gms. at 100**.
(Tarugi and Cbecchi, x9ox.)
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.
100 cc. 95% alcohol dissolve 0.00136 gm. CaC4H404.HiO at 18"* and 0.00136 gm.
at 25^. (PUheil and Habner, X903.)
CALCIUM SUIiTATE
214
CALCIUM SULFATE CaS04.2H,0.
Solubility in Water.
(Hulett and Allen, XQ02; for references to other detemninatiom aee Hulett
For data by the electrolytic conductivity method^ tee WwiUw**!*, Kohlnuuch
and AUen, also Enkr. 1904*
and Roae, 1893, 1908.)
f.
O
10
18
30
35
Gms. CaSOi
per xoocc
Solution.
O.I7S9
0.1928
0.2016
0.2080
0.2090
0.2096
Millimols
per liter.
12.926
14.177
14.817
15-361
15-405
Density of
Solutions.
I. 00197
I. 00173
1.00059
O.999II
0.99789
0.99612
40
55
653
75
100
107
Gms.CaS04
per xoocc
Solution.
0.2097
0.2009
0.1932
0.1847
O.1619
Millimnli
per liter.
15-413
14-765
14.200
13.575
11.900
11.390
Density of
Solutions
0.99439
0.98796
0.98256
0.97772
Solubility of Calcium Sulfate Anhydrite and of Soluble Anhydrite
IN Water. (Mdcher, 19x0.)
f.
100
100
100
156
156
218
Millimols i)er
Liter.
11.65
II. 4
4.6
3-2
1-35
0.35
Gms. CaSOiper
Liter.
1.586
1-552
0.626
0.436
0.184
. 0.048
SoUd Phase.
CaS04.2H20
Soluble anhydrite
Anhydnte
Soluble anhydrite
Anhydrite
Data for the solubility'of calcium sulfate in sea water are given by Manuelli, 1916.
Solubility of Calcium Sulfate in Aqueous'Solutions of Akiconium
Acetate at 25**. (Mardenri9i6.)
Gms. CHsCOONHi per
100 Gms. Solution.
dn.
Gms. CaSOi oer
zoo' Gm5. Sat. Solution.
0
I
0.2085
2.13
1.005
0.454
5-34
1. 012
0.752
10.68
1.024
1. 146
21.37
I.04S
1-755
Solubility of Calcium Sulphate in Aqueous Solutions of Hydro-
chloric, Nitric, Chlor Acetic, and Formic Acids.
(Bantbisch — J. pr. Chem. ag* 53. '84; Lunge — J. Soc. Chem. Ind. 4, 3a, '85.)
In Hydrochloric.
Grams Add
per xoo cc.
Solution.
O
I
2
3
4
6
8
10
12
Grama CaSO« per
100 cc. Sol.
at as°'
0.208
0.72
1.02
1-25
1.42
1.65
1.74
In Nitric. In Chlor Acetic. In Formic.
Gms. CaSO« per Gms. CaSOa per Gms. CaSO« per
xoo cc- Sol.
atioa*.
0.160
1.38
2.38
3.20
sM
4-65
100 cc. Solution
at as"*.
atai*.
0.208
xoo cc. Soi.
at as°.
208
0.208
0.56
0.82
1.02
1.20 0.22 0.24
1.48
1.70
1.84 0.25
1.98
Data for the solubility of mixtures of CaS04(NH4)» SOi.HjO + (NH4)»S04 and of
CaS04(NH4)aS04.4HiO + CaS04.2HiO at various temperatures between 3** and lOO*
are given by Barre, 1909 and 191 1. Additional data for this system, including re-
sults for the pentacalcium salt, (NH4)sCai(S04)6.HsO, are given by D'Ans, 1909.
215
CALCIUM SULFATE
SoLUBiLrrY OF Calcium Sulfate in Aqueous Solutions of Ammonium
Salts.
(In tJH^ and NH«NO», Cameron and Brown — J. Physic. Chem. 0, axo. '05 ; In (NH«)9S04 at 95*,
SdUyan — J. Am. Chem. Soc. a7f 599t '05; In (NH4)9S04 at 5o^ Bell and Tabor — J. Physic. Chem. 10,
"'^ "^'^ In NH,C1 In NH,NO, In NH,C1 In NH4NO,
at 25^.
at
25^
at 25^
at 25**.
niumSak
G.CaSO*
Dissolved
G. CaSO*
Dissolved
Gms. Ammo-
nium Salt
G.CaSO^
Dissolved
G.CaSO*
Dissolved
per Liter.
per liter.
per
Uter
per Liter.
per Liter.
per Liter.
0
2.08
2
.08
300
10. 10
10.80
20
500
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
12.10
ICO
9.10
7 65
1000
II. 81
150
10.30
8.88
1400
10.02
200
10.85
9
8s
sat
7-55
In (NHJsSO, at 25^.
In (NHJ^SO, i
at 50**.
Grams per
Uter Sol. wt. of loo CC
•
Grams per
Liter Sol.
Sp. Gr.
(NH4}sSO«.
CaS04.
Sat. Sol.
(NH4),S04.
CaSO*.
of Solutions.
0
2.08
99.91
0
2.168
• • •
0.129
2.04
99.91
15-65
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
I 643
1.66
99-99
160.4
3.402
I. 0819
3.287
1-54
100.10
221.6
4.068
I.II08
6. 575
1.44.
100.34
340.6
5.084
I -1653
13 15
1.46
100.82
416.5
5-354
I. 1964
26.30
1.62
101.76
428.4
4.632
1 . 2043
84.9
2.33
105.34
530.8
2.152
I - 2437
169.8
3-33
110.32
566
1.08
1.2508
.339-6
4.50
119. IS
566.7
0
1.25x0
In Calcium
Nitrate.
Gms. per Liter Sol.
SoLUBiLiTT OP Calcium Sulfate in Aqueous Solutions of Calcium Salts
AT 25*
(Csmeroa tnd Seidell — J. Physic. Chem. S» 643, '01; Seideil and Smith — Ibid. 8» 493, '04; Cameron
and Bell — J. Am. Chem. Soc. aS» laio, '06.)
In Calcium
Chloride.
Grama per Liter Sol. ums. per .uter Soi. wt. of
CaOi. CaSOP Ca(NOj)a. CaSO*. i cc.'Sd.
0.00 2.06 0.0 2.08 0.998 0.0
7.49 1.24 25 1.24 1. 014 0.062
11.96 I. 18 50 1.20 I. 032 0.176
25.77 I. 10 100 I. 13 1.067 0.349
32.05 1.08 200 093 1. 137 0.61
51.53 1.02 300 0.76 1.204 0.939
In Calcium Hydroxide and
vice versa,
Gms. per Liter Sol.
daOT ^
97
192
280
367
02 0.84 400 0.57 I
71
30
85
047
0.20
0.03
500
544
0.40
0-35
I
I
CaS04.
2.126
2.030
1. 918
1-853
1.722
1.634
Solid
Phase.
CaS0..2H,0
It
It
tt
u
265
328
352
1.222
1.242
1.150
1. 166
^r^ [ CaS0,.2H,0+
•5^ ( Ca(OHj,
1. 2 14 Ca(OH),
0.666
0.00
CALCIUM 81JLFATI
3l6
Solubility op Calcixtii Sulfate in Aqueous Solutions of Copper Sulfate
AT 25'.
(Bell and Taber, 1907.)
Cms, per Liter Sat. SoL
CuSOi.
1. 144
3 564
6.048
7.279
14.814
19.729
29 543
CaSOi.
2.068
1.986
1.944
1.858
1.760
I 736
1.688
daSatSoI.
1.002
1.005
1.007
1.009
1. 016
1. 021
1.030
Gnus, per Lit*r Sat. Sol.
CuSOt.
39 407
49 382
58.880
97 950
146.725
196.021
224.916
CaSOi.
1. 718
1.744
1.782
I 931
2.048
2.076
2.088
d« Sat. Sol.
1. 041
1. 051
1. 061
1.098
1. 146
1. 192
1. 218
Solubility of Mixtures of Calcium Sulfate and Caesium Sulfate in
f.
25
60
Mo]8.CaiSOi.CaSOi
per xooo Gms.
Sat. SoL
0.667
0.607
Water.
(D'Aas, 1908.)
Gms. CasSOi.CaSOi
per Tooo Gms.
Sat. Sol
352
320
Solid Phase.
Dicaldum Sulfate + Gypsum
U It
Solubility of Calcium Sulfate in Aqueous Solutions of Magnesixtm
Chloride and of Magnesium Nitrate at 25^
In Magnesium Chloride.
In Magnesium Nitrate.
Grams
per Liter of Sat.
• 1
Solution.
Grams per
Liter Solution.
Wt. of z cc.
MgOs.
CaSOi.
IW).*
MgCNOOs.
CaSOi.
Solution.
0 .
2.08
997-9
0
2.08
0.9981
8.50
4.26
996.5
25
5-77
1.0205.
19.18
5 69
994.5
50
7.88
1.0398
46.64
7.59
989.1
100
9.92
1.0786
121.38
8.62
972.2
200
13.34
I . 1498
206.98
6.57
949.9
300
14
I. 2190
337
2.77
908.7
400
14.68
I. 2821
441. 1
1-39
878.6
514
15.04
1.3553
LUBILITY
OF Calcium Sulfate in
Aqueous Solutions of
Magnesium
Sulfate
AT 25*.
(Cameron and Bell, x9o6a.)
Grams per Liter Solution.
Sp. Gr. of
Gramnper
Liter Solution.
Sp. Gr.'of
MgSOi.
Casa.
Solutions at If*.
MgSOi.
CaSOi.
Solutions at H*-
0
2.046
1.0032
149.67
1.597
I. 1377
3-20
1.620
I .0055
165.7
1.549
I . 1479
6-39
1.507
1.0090
171. 2
1-474
1. 1537
10.64
1. 471
I.OI18
198.8
1.422
I.1813
21.36
1.478
7.0226
232.1
1.254
1.2095
42.68
1.558
I. 0419
265.6
1.070
I . 2382
64.14
1.608
1.0626
298
0.860
I . 2624
85.67
1. 617
1.0833
330.6
0.647
1.2877
128.28
1.627
I.II90
355
0.501
1.3023
217
CALCIUM 8ULFATI
Solubility of Calcixtii Sulfate in Aqueous Solutions of Phosphoric
Acid at 25®.
(Taber, 1906.)
Cms. perl
Liter.
Sp. Or. of
SdutioDs at H
•
Cms. per Liter.
Sp. Gr. of
P^
CaSOi.'
P«0». CaSa.
Solutions at H.
0
2.126
0.9991
145. I 7.920
1. 106
5
3-143
1.002
205 8.383
1. 145
10. 5
3-734
1.007
311. 5 7.965
1. 221
21.4
4.456
1. 016
395.8 6.848
1.280
46.3
5-760
1-035
494.6 5.572
1.344
105.3
7.318
1.075
■
Solubility of
Calcium Sulfate in j
\queous Solutions of Sulfuric Acid.
(Cameron and Bieaseale, 1903.)
Grams HtS04
Results at af.
Results at 3^. Results at 43^.
Gms. CaS04 Gms. CaSQA
per Liter of
Gms. CaSO^ Wt. of ]
[ cc.
Sdutioa.
per Liter.
Sol.
per Liter.
per Liter.
000
2.126
0.9991 grams ...
2-145
0.48
2.128
1.0025
2.
209
2.236
4.87
2.144
1.0026
2
451
2.456
8. II
2.203
1.0051
» • •
2.760
16.22
2.382
1.0098
» ■ •
3-I16
48.67
2.727
1 .0302
3
397
3 843
75 00
2.841
I 0435
t m •
4.146
97-35
2.779
I .0756
3
606
• * •
146.01
2.571
• • •
3
ISO
4 139
194 70
^'3^3
1.1134
t 1 •
3 SSI
243-35
1. 901
1.1418
• • «
a -959
292 .02
I -541
1.1681
t
1 • •
a. 481
Solubility of Calcium Sulfate in Aqueous Solutions of Potassixtm
Chloride, Brobode, and Iodide at 21°.
(Ditte, 1898.)
In KCl Solutions. In KBr Solutions. In KI Solutions
Giamsof the
PotasdumSalt
per Liter.
O
10
20
40
60
80
100
"5
ISO
200
250
300
Cms. CSO^
per liter.
Gnu. CaSOk
per liter.
Gms. CSO^
per liter.
2.05
36
2 OS
31
2.0s
2.8
4S
3-6
33
S-8
6.6
4S
S-2
3 9
45
7.2
S-9
4-85
7S
double salt
6-3
6.7
S-i
S-4S
• • •
7.0
S-8
• • •
« • •
7-3
double salt
5 -95
6.0O
• • •
• . 1
double salt
CALCIUM 8ULFATI
218
Solubility of Calcium Sulfate in Aqueous Solutions op Potassium
Nitrate and of Potassium Sulfate at 25**.
(Seidell and Smith, 1904; Cameion and Breaseale, 1904.)
In Potassium Nitrate.
In Potassium Sulphate.
Gma. per liter
SohxtioD.
Wt.of IOC.
Sdatioii.
KNOi.
CaSO«.
0.0
2.08
0.9981
"S
3 28
I. 0081
25.0
4.08
I .0154
50.0
5-26
I. 0321
.100.0
6.86
1.0625
ISO
7.91
1.0924
200
8.69
1. 1224
260
syngenite
1 1539
Gms. per Liter
Solution.
0.0
4.88
S09
9-85
I9S7
28.35
30.66
32.47
CaSOi.
2.08
60
S6
45
49
SS
57
58*
Wt. of I oc.
SolutioQ.
0.9981
1.0036
1.0038
1.007s
I 0151
I .0229
1.0236
* Solid phase sjmgenite. Results for the solubility of syngenite in aolatioos of potassiom sulphate aie
also given in the anginal paper.
Data for the solubility of syngenite, KtCaCSOOs.H^O, and of potassium pentacal-
cium sulfate, K2Ca((S04)6.HsO, in water at various temperatures, are ^ven 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**: KCl, KBr, KI, KCK),. KCIO4. KNO,, CH,C06k, KOH, K4Fe(CN).
K,Fe(CN)6, NaCl, Nal, NaNOs, CH,CCX)Na, HCl, HNO,. HjPO*. CH,COOH,
HsSOi, AgiSOi and cane sugar.
Data for the solubility <5 mixtures of CaSO^^KoSOt.HiO + CaSO«.2HaO and
CaSO4.KsSO4.H1O + K2§04 in_water at temperatures between o® and 99", are
given by Barre (1909, 191 1).
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).
S(H.UBILITY OF CaLCK
(Cameron, 1901
Grams per zoo cc. Solution.
ni Sulfate »
CH1.0RIDE
; also Orloff, 1903;
Wt. of X cc
Solution.
0.9998
1.0644
I. 0981
I.IOI2
r Aqueous Solutions of
AT 26^
Cloez, 1903; d'Anaebne, 1903.)
Grams per xoo cc. Solution.
SODIUH
Wt. of I oc.
NaCl.
0
9. IIS
14-399
14.834
CaSOi.
0.2I2I
0.666
0.718
0.716
NaCl.
17.650
22.876
26.417
32.049
CaSO«.
0.712
0.679
0.650
0.572
Solution.
I.II96
I. 1488
1. 1707
1.2034
Solubility of Mixtures of Calcium Sulfate and Calcium Carbonate in
Aqueous Solutions of Sodium Chloride at 23^
(Cameron and Seidell, z9oza.)
Gm
ms per Liter Solul
Lion.
(Srams
per Liter SolutlOB
t.
Naa.
0
3-^3
11.49
39.62
Ca(HCOi)t.
0.060
0.072
0.089
O.IOI
CaSOi.'
1.930
2.720
3.446
5.156
NaCl.
79. 52
121.90
193.80
267.60
Ca(HC0i)i.
0.060
0.056
0.048
0.040
CaSO^
6.424
5.272
4.786
4.462
Data for the solubilitv of mixtures of calcium sulfate and sodium chloride at
0^-09® are given by Artn and Cretien (1906).
Data for the equilibrium CaS04 + NaiCOi <Fi CaCO» + NasSOi at 25* are
given by Herz (1911a).
219
CALCIUM SIJLFATK
Solubility of Mixtures of Calcium Sulfate and Silver Sulfate in
Water.
CEuler, 1904.)
^ . ( CaS04
'7 {Ag,S04
Gnis.Salt.
2-31
7 -235
Per Liter of Solution.
Gms. Equiv.
Salt.
^^o(CaS04 2.61
^5 {A&SO4 8. II
0.034 )
0.0464)
00383)
0.0520 )
Total Sah
per xoo Gms.
SolatMm
0-9473
1.062
Sp. Or. of
SdtttioDs.
1.0083
1. 010
'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. wt. of z oc
Gms. per Liter Solution. wt. of r cc
NaNOi. CaSOi. ^ Solution.
'NaaSa.
CaSOi: Solution.
0 2.08 0.9981
2.39
I. 65 I. 0013
25 4.25 I. 0163
9S4
I. 45 1.0076
SO 5 SO I 0340
14.13
1.39 i.oiis
100 7.10 1.0684
24.37
1.47 I.020S
200 8.79 1. 1336
46.15
1.65 I. 0391
300 9 . 28 1 . 1916
11508 •
2.10 1.0965
600 7.89 1.3639
146.61
2.23 I. 1427
65s 7 24 1-3904
257.10
2.65 I. 2120
Data for the solubility of calcium sulfate, sodium sulfate glauberite, sodium
sulfate synffenite. separately and mixed, in water at various temperatures, are
given by D Ans (1909) anc^Barre (191 1).
Scmlubility of Calcium Sulfate in Aqueous and Alcoholic Mono-
potassium Tartrate Solutions at 20^.
(Magnanini, 1901.)
Solvent.
Water
Aq. N/200 KHC4HA
10% alcohol
Gms. CaS04
per 100 Gms.
Solution.
0.2238
0.2323
0.0970
Solvent.
10% alcoholic N/200 KHCAOi
Aq. N/200 KHC^0»+5% tar-
taric acid
10% ale. N/400 KHCJIiO.+s%
tartaric add
Gms.CaS04
per xoo Gms.
Solution.
0.0866
0.2566
0.1086
Solubility of Calcium Sulfate in Aqueous Sugar Solutions.
(StoUe, z9oa)
Per cent Concen-
tration of Sugar
Solutions.
Gms. CaS0« Dissolved by zoog
Gms. of the Sugar Solutions at:
r-
30-.
40*.
so*.
6o*.
70*.
8o*.
0
• • •
2.157
I 730
1.730
1.652
1. 710
10
2.041
1.730
I 730
1. 574
1.574
1. 613
20
1.808
1.652
1. 419
1.380
1.419
1.263
27
^•SSo
1.438
1. 361
1.283
1.283
0.972
35
1.263
1.050
1.088
1. 108
0.914
• • •
42
1.030
• • •
0.777
0.816
0.85s
0.729
49
...
0.564
0-739
0.564
0.603
0.486
ss
• . •
0.486
0.50s
0.486
0.369
0.330
1 00 gms. glycerol of du ^
[.256dissolv
e 5. 1 7 gms
.CaS04ati5°
-16**. (088endow!iki,igo7.)
100 gms. glycerol oidi
.1 14 dissolve 0.95 gm.
CaSOi at ord
. temp.
(Asselin, 1873.)
CALCIUM SULFATI 220
Freezing-point Data (Solubilities, see footnote, p. i) Are Given for the
Following Mixtures of Caluum Sulfate and Other Salts:
Calcium Sulfate + Lithium Sulfate (Muller, 19x0.)
+ Potassium Sulfate (Mailer, 19x0; Gnhnuum, 19x5.)
+ Rubidium Sulfate (Muller, 19x0.)
4- Sodium Sulfate (MOlkr, 19x0; Calca^ni and Mandni, Z9ia)
41 41
11 II
II II
OALOIUM SULPHIDE CaS.
Solubility in Aqueous Sugar Solutions.
(StoUe.)
tnJdaaci Sugar
SoltttioDs.
Grams CaS DiaaolTed per Liter of the Sugar Solutions at:
»
»
Soo.
40».
50«.
6o<».
ro^
&>•.
90 .
0
1.982
2.123
1-235
I 390
1.696
2.032
2.496
10
1.866
1. 316
1. 441
1-673
1.560
1-634
1-544
20
2.187
1.696
1.802
1-905
1.879
1.892
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
2.818
3 063
55
2.509
2.226
2.340
2.882
2.766
2.972
3 -616
CALCIUM SULTITE GaSOs2HsO.
Solubility in Water and in Aqueous Sugar Solutions at i8^
(Weisbexg. X896.)
Grains CaSOi per 100 cc. Solution.
Solvent. AtTft* 'After Boiling
At " . Solution a HouxB.
Water 0.0043
10 Per cent Sugar o . 0083 o . 0066
30 Per cent Sugar 0.0080 0.0069
Results at Higher Temperatures.
(Van der Linden, 19x6.)
Gms. CaSOi.aHsO per xooo gms. Sat. Solution at.
Solvent. r- "^ \
30*. 40*. so*. 6o*. 70*. 8o*. 90*. b. pt.
Water 0.064 0.063 0.057 0.061 0.045 0.031 0.027 0.01 1
Aq^Sucroseofi5gms.pcrioo 1^^^^ ^^^ ^^^^ ^^ ^^^^ ^^^ ^^^^ ^^^
'^G£^F;e;^rcc1"''''^^ -^^ ^-^5 0.071 0.060 0.047 0.040 0.029
Water+Excess CaSOi 0.031 0.029 0.025 0.019 0.012 0.009 0.008 0.006
%^Ex'i^'(^^*^'''^^"}^-°3S 0.032 0.022 o/>i9 0.021 0.017 0.020 0.021
Aq. Sucrose, 15 gms.+i.5 gms. 1
Glucose per 100 cc+Ezcess ( 0.032 0.027 0.022 0.020 0.019 0.0x9 0.019 0.033
CaSO* '
CALCIUM Phenanthrene SULFONATES.
Solubility in Water.
(Sandquist, x9xa.)
Caldiun- 2-Phenantlirene Monosulfonate 0.034
" - 3- " " .2IWJ 0.083
" -10- " " .2HiO 0.30
Gms. CliC4HiO|.4EI^
per loo cc. SoL
f.
Gms. CaCiHiO^i^bO
per xoo cc Sol.
f.
Gms. CaGH<(>|.iHiO
per 100 cc. SoL
•0.0365
30
0.0631
70
0.1430
0.0401
40
0.087s
80
0.1798
0.047s
SO
O.IIOO
«s
0.2190
0.0525
60
0.1262
221 CALCIUM TABTRATI
CALCIUM TABTRATI CaCdi^fkAHfi.
SoLUBiuTY IN Water.
(Ctntoni and Zschoder, 1905-)
o
10
20
100 ems. aq. Ca. tartrate solution contain 0.0185 gm. CaC4H40c4HiOat 18^, and
0X)294d9 gm. at 25^.
100 gms. 95% alcohol solution contain 0.0187 gm. CaC4H40«.4HsO at 18^, and
0.02352 gm. at 25®. ^ (PartheQ and HObner, 1903.)
100 gms. aq. Ca. tartrate solution contain 0.0364 gm. CaC4H40« at 20**.
100 gms. 10% alcohol solution contain 0.0160 gm. CaC4H40« at 20^.
100 gms. aqueous 5% tartaric acid solution contain 0.1632 gm. CaCiHiOs
at 20°. (Magnanini, 1901.)
Scx^ubhity of CALaxTii Tartrate, CaC4H40c4H«0, in Aqueous Acetic
Acid Solutions at 26*-27".
(Hers and Muhs, 1903; see also Enell, 1899.)
NonnalityoC Gms. CHiCOOH Residue from Normality of Gms. CHaCOOH Residue from
Acetic Acid. per xoo cc. SoL 50.05a cc. Sol. Acetic Add. per xoo cc Sol. 50.052 oc. SoL
o o 0.0217 3.80 22.80 0.2042
0.57* 3.42 0.1082 S.70 34.20 0.1844
1-425 8.55 0.1635 10.09 60.54 O.II60
2.85 17.10 0.1970 16.505 93.03 0.0337
The residue was dried at 70^ C.
S(x«UBiLiTY OF Calcium Tartrate in Aqueous Solutions of CALauii
_, Chloride, Tartaric Acid, etc., at 18".
(Paul, X9XS.)
(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 COt in the water had a distinct influence on the solubility. One
liter of pure COt free water was found to dissolve 0.380 rtn. CaC4H40c.4HtO at
18° and one liter of ordinary distilled water, 0.410 gm. at the same temperature.)
Results for Aque- Results for Aqueous Results for Ague- Results for Alcoholic
ous Calcium Dipotassium Tar- ous Tartaric Tartaric Acid
Chloride Solution. trate Sols. Acid Sols. Sols.
' Gms. per Liter. Gms. pex
Liter.
CadHiO;.
4IUO.
Gms.
per Liter.
Gms. per Liter.
CaOt.
CaC«HiOi. KfiaH«Oi.
4HSO. iHsO.
CiHiOk
CaC4H40^
4HiO.
CtTWH.
CdWt.
CaC«H4d^
4H1O
0.503
0.202 0.392
0.166
I
0.910
SO
0
0.263
1.005
0.179 2.139
0.160
2
1. 162
it
4
1. 107
3518
0.166 2.352
0.157
4
1.5"
u
16
1.85
4 523
0.154 2.614
0.150
6
1.776
80
0
0.205
5.025
0.154 4.705
0.223
8
1.972
((
4
0.867
7.538
O.171 23.524
0.263
10
2.205
tt
16
1.506
10.05
0.177 47.048
0.305
12
2.380
100
0
0.190
25x25
0.182
14
2.514
«
4
0.766
50.25
0.224
16
2.643
tt
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 TABTRATI
333
Solubility of Calcium Tartrate in Aqueous Solutions of Aioionium,
Potassium and Sodium Chlorides at Several Temperatures.
(Ctntoni and Jolkowiky, 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.)
Gms. Chloride per
Liter Solvent.
S
10
30
100
200
Gms. Ca Taztnte Dissolved at
16* per Liter of Aq.:
NH4a.
0.701
0.861
1. 281
1.897
2-305
Ka.
0.643
0.822
1. 180
I -753
2. no
NaQ
0.680
0.840
1-305
1.860
2.163
f.
16
30
55
70
85
Gms. Ca Taztimte per liter of
7% Aqueous:
NH4a.
1.676
2.417
3-712
5.080
6.699
KCl.
1.504
2.031
2.154
2.546
4.264
NaQ.
1.637
2.275
3-579
4.148
6.305
OALOIUM BITABTBATE CaH.CC^H^Oe),.
Solubility in Water and in Aqueous Solutions op Acids and
OP Salts.
(Warington — J. Chem. See. aS, 946, '75.)
In Hydrochloric Acid. In other Acids and in Salt Solutions at 14**.
Cone, of HCl
Gms. per
zoo Gms. Sol.
O
0.68
2-15
4.26
8.36
16.13
Gms. CaH|(CiILOa)a
per zoo Gms. Solvent.
At aa**.
0.600
3.01
6.88
1 1. 19
22.7s
48.31
At8o«.
4.027
5-35
20.23
40.93
80.12
xoo
sms. HfO dissolve o^ps gms«
bitartrate at 14"
Add or Salt.
Gms Add or Salt Gms. CaHfl(CJB[«Ob)s
per xoo cc. Sol.
Acetic Acid
Tartaric Acid
Citric Acid
Sulphuric Acid
Hydrochloric Acid
Nitric Acid
Potassium Acetate
Potassium Citrate
per zoo cc. Sol.
0.81
1.03
0.84
0.685
0.504
0.845
1.387
1-397
0.422
0.322
0.546
1. 701
1.947
1.969
0.744
0.843
CALCIUM THI08ULFATE CaSAeHsO.
Solubility of Calcium TmosuLFATE in Aqueous Solutions op Sodium
ThIOSULFATB at 9** AND 25" AND ViCE VERSA.
(Kremann and Rodemund, 19x4.)
Results at 25^
Gms.
Results at 9^
xoo Gms.
KaaSiOi.
O
11.04
25.21
31 01
t. Sol.
Gms. per xoo Gms.
Solid Phase.
CaSiOi.
29.4
22.64
15-84
CaSsQs.6H^
. per
Sat.Sol.
«
o
"+Na«S,Os.sEM) 15.67
7.70 Na«SiOj.5H20
CaSi0%
34.7
29.69
21.41
25.18
21.14
20.33
Solid Phase.
CaS|Q8.6HaO
«
(C
tt
18.34
28.24
30.19
31-24
35 04
Data are also given for the quaternary systems, CaS|0|-HNa»SjOs-hNaNQi
+H,0 and CaS,0,+Ca(NO,),+NaNO,+H,0 at 9** and 25^ A triple salt of the
composition CaNa«(S«Oi)sNOi.iiHiO was obtained.
"+NaAQ..sHiO
18.43 NatSsOa-sHaO
II. 61
((
223
CALCIUM VALEKATE
OALOIXTM VALERATE Ca[CH,(CH,),COO],.H,0.
CAI.OnrM (Iso) VALERATE Ca[(CH,),.CH.CH,.C00],.3HA
Solubility op Each in Water.
— J. Chem. S0C.81, 355, '02; see also Furth — Monatsh. Chem. 9, 313. *88; Sedlitaky—
Ibid, 8, 566, '87.)
%\
Calcitam Valerate.
Cms. Ca(G^l0Qt)a
per zoo Gms.
Calcium Iso Valerate.
Cms. CaCCftHoOa)!
per 100 Gms.
O
10
20
30
40
SO
57
60
70
80
90
100
Water.
9.82
9-25
8.80
8.40
8.05
•85
SdotioD.
8.94
•75
.78
.80
•95
8.20
8.78
8
8
7
7
7
7
7
7
7
7
8
o
10
20
30
40
45
50
60
70
80
90
100
Water.
26.05
22.70
21.80
21.68
22.00
22.35
19 95
18.38
17.40
16.88
16.65
16.55
t(
tt
IC
tt
Ca(C,H.O,),.H,0
47
09
75
45
28
19
22
24
36
58
.07
CAMPHEME CioHtt.
Freezing-point data (solubility, see footnote, p. i) are given by Kumakov and
Efrenov (1912) for mixtures of camphene + methylmustard oil, caniphene+
naphthalene and camphene + phenantnene.
CAMPHOB CuiHieO ^ and /.
^PROXIMATE Solubility of d Camphor in Several Solvents at Ordi-
nary Temperature. (U. S. p., Squires; Greenish and Smith, 1903.)
Parts Camphor per
Solution.
20.66
18.50
17.90
17.82
18.18
18.42
16.63
1552
14.82
14.44
14.28
14.20
Solid
Phase.
Ca(C.HyO,)r3H,0
tl
tt
(t
it
Solvent.
Water
90% Alcohol
95% Alcohol
Ether
Parts Camphor
per zoo Parts
Solvent.
0.08-0.14
100
125
173
Solvent.
Chlorofonn
OUve Oil
Turpentine
Glacial Acetic Acid
kono
xoo Parts solvent
300-400
25-33
66
200
12.5 (Kl08e,x9O7)«
CaxboQ Disulfide Readily Soluble Lanolin
Saturated solutions of d camphor and of / camphor in turpentine of an 74.38
(in a 10 cm. tube at 18**) were found to have (/it— 0.9028 and 0.9030 respectively;
the 02) 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
readue on account of volatilit}^; polarimetric methods could not be used on account
of the interference of the H(Jl. The author, therefore, determined the densities
(HsO 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 prepar^ by stirring the several mixtures with a glass
stirring rod, at intervals, during 6 hours.)
Solvent. "
Densities at 0".
Densities at 10*.
Densities at 20*.
Densities at 40*.
Solvent.
Sat. Sol.
Solvent. Sot. Sol.
Solvent. Sat. Sol.'
' Solvent. Sat. Sol. '
27.2 %HC1
1. 145
1. 143
I . 140 I . 138
I. 135 1.133
I. 153 1.148
I. 125 1.12^
I . 142 I . 131
30.6 "
1. 164
I 159
I. 158 I. 153
339 "
1. 181
1. 167
I. 175 I. 163
I. 169 1.159
I. 175 1 158
1.157 1.149
1.163 I. 153
34.98 "
1. 187
1. 158
I. 181 I. 160
35.74 "
1. 191
1. 140
I . 185 I . 148
I 179 1 153
1.167 1.153
3^'3S '
1.195
1. 126
I. 189 1.134
I. 182 1.140
1. 170 1. 153
36.68 "
1. 197
1. 1x6
I. 190 I. 124
1 . 184 1 . 134
... ...
CAMPHOR
224
Reciprocal Solubilitt of Camphor and Phenol, Dbtbrminbd 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.
,
Gms.
fof
«?
Camphor
SoUd
fof
Camphor
Solid
fof
Camphor c^ijj
Frew-
ing. (
per ICO
Sms. Mix-
ture.
Phase.
Freezing.
per 100
Gms. Mix-
ture.
Phase.
Freezing.
ture.
174. S
lOO.O
C»Htf0
-13.8
71.48 C»Hi^
— 22.6
52.52 X.l
158
95.98
It
-26.4,-
32 70.12
" 4-1. X
— 23.6
44.90 "
140
92. ss
M
-15. 9
69.32
x.z
- 28-30. s
40.3s "+C.a0H
112
88.86
t(
— 20.1
67.76
M
-157
38.57 CJI.0H
80
82.88
l(
-19.3
66.64
<•
-3
34.50 "
SO. 7
79.73
If
— 18.7
62.21
If
+S
30.31 "
29.5
76.58
l<
—18. 6 m.
pt. . . .
M
16. 1
25.40
— o.i
73-37
II
—20.1
61.51
M
25
20.31 "
-135
72.24
M
— 20
SS.80
M
36.1
6.87 «
I.I =
Ci
cHwO.CeHsOH.
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 (19 15). The results are not in good agreement with the above. These
authors also give similar determinations for the systems camphor -f-resordnol and
camphor +^ naphthol.
Data for the systems camphor + phenol -f- water, camphor -|- n butyric add -H
water, camphor -f- succinic acid nitrile + 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 + Bomeol
-j- Hydroquinone
4- Menthol
+ a Naphthol
-f- fi Naphthol
+ a Mononitronaphthalene
-j- Naphthalene
-f- /S Naphthylamine
it
(I
«
(Vanstone, X909.)
(Efremov, X9X3, X9X3.)
(Pawlewski, 19x3.)
(Caille. 1909.)
(Caille, X909.)
Qoumiauz, X9xa.)
II
11
i<
II
II
II
II
II
II
II
it
II
(I
+ Nitric Acid
-j- Phosphoric Acid
4- Pyrocatechol
4- Pyrogallol
+ Resorcinol
+ Said
+ Sulfur Dioxide
-j- a Trinitrotoluene
-f- p Toluidine
+ 17 other compounds
(Zukowand
II
i«
1909.)
(Efxemov, 191 a, 19x3.)
Qoumiauz, x9xa.)
(CaiUe, 1909; Efremov, X913, I9I3-)
(CaOfc, X909.)
(Bellucd and Gnasi, X913, X914.)
(Giua, 19x6.)
(Efremov, X9X5« 19x6.)
BenzolGAMPHOR Enol and keto forms.
Solubility data have been used by Dimroth and Mason (191 3) 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 freeang-
point metfiod. (Sidgwkk, 191$^
235 BromoCAMPEOR
BromoCAMPHOR aCioHuOBr.
Approximate Solubility in Several Organic Solvents at Ordinary Temp.
(U. S. p.; Squires; Betlstein; results in alcohol by Mttller, 1893.)
« , » Parts Bromo Camphor c^i„*«* Parts Bromo Camphor per
Solvent. per 100 Parts Solvent. Solvent. 100 Parts Solvent,
Alcohol i2.iati5** Ether S^
" 19.7 " 25® Chloroform 143
" 130.0 " so** OUveOil 12.S
" 705.0 " 61** 95% Formic Acid 13.6 (Asdam, 1913.)
Freezing-point data (solubility, see footnote, p. i ) are given for mixtures of I bromo-
camphor ■+• d chlorocamphor by Padoa (IQ04) ; for mixtures of d bromocamphor-h
/ bromocamphor by Padoa and Rotondi (1912); for mixtures of bromocamphor -|-
Btearine by Batelli and Martinetti (1885); /3 bromocamphor + salol by Caille, 1909.
CABfPHOROXIME CuHieiNOH Jand /.
100 gms. turpentine dissolve 8.68 gms. d oxime at 18^, du == 0.8784, oed « 2.30
in 10 cm. tube.
100 gms. turpentine dissolve 8.69 gms. I oxime at l8^ du^ 0.8782, od ^ 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 I amyl bromide the dn « i'i99 in both cases and the
ap was —3.55 (10 cm. tube) for the d oxime and + 1 1.48 for the / oxime. The ao
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 I isomerides are identical in an optically
active as well as in an mactive solvent.
Freezing-point data are given for mixtures of d and / camphoroxime by Beck
(1904) and Adriani (1900). "^
CABfPHORIC ACm C8Hu(C00H)s.
100 gms. of water dissolve 0.8 gm. CsHuCCOOH)] at 25**, and 10 gms. at the b. pt.
SdusBTLvn OF Camphoric Acid in Aqueous Solutions op Alcohol at 25*.
(Seidell, 1908, xgio.)
Wt. % CtHiOH dm of Gms. C JIi«(COOH)s Wt. % CsHiOH d» of Gms. CaHu (COOH)i
in Solvent. Sat. SoL per xoo Gms. Sat. Sol. in Solvent. Sat. Sol. per xoo Gms. Sat. SoL
o I 0.754 60 I 4S
10 I 1.60 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.
imcA Gms. im^ Gms.
Solvent. r. Sat. CsHi«(COOH)s per Solvent. t*. Sat. CsHu(C00H)tper
Sol. xoo Gms. Solvent. Sol. xoo Gms. Sdvent.
Amyl Alcohol(iso) 25 0.907 50(3) Carbon Disulfide 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).
(x) Timofeiew (X914); (3) Beilstein; (3) Seidell (19x0); (4) Ascban, (X9X3).
Data for the distribution of camphoric acid between water and ether at 25° are
given by Chandler (1908). Data for the freezing points of mbctures of d and /
camphonc>cid and d and / isocamphoric acid are given by Centnerszwer (1899).
CAMPHORIC ANHYDRIDK CioHuOt i and /.
One liter of benzene dissolves 37.5 pns. d camphoric anhydride at 5*, deter-
mined by depression of the freezing-pomt. (Sidgwick, x9x5.)
« «
CANTHABIDINS 226
Appkoxiuate Solubilitt in Several Solvents at Room Temp.
(Sdf ftnd Greenish, 1907.)
Gms. Cantharidine Gma. Cantharidine
Sdvent. per zoo Gms. Solvent. per zoo Gms.
Solvent. Solvent.
Aq. 25% Acetone 0.02 Aq. 10% Acetic Acid 0.14
" 50% " 0.16 " 45% Formic " 0.12
" 75% " 0-4S Carbon Tetrachloride 0.04
Lanolin 4.4 (Kiose, 1907.)
CAOUTCHOUC.
Solubility in Organic S(h.vbnts. (Hanausek, xSSt.)
Gms. Caoutchouc Dissolved per xoo Gms. Solvent.
Solvent. / * \
Gears. 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 Disulfide 0.4 o o
SoLUBiLrrr of Caoutchouc in Mixtures of Benzene and Alcohol. (Caspan. zgis)
(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®.
Caoutchouc. *** ^^*^ &U0JL CaoutSouc ^' ^^ SbSoH. CaouSouc. "' ^^^- ^Olf.
0.032 40 17 0.206 40 II 0.80 40 9.6
0.080 40 15.8 0.81 40 10.8 2.01 40 8.8
0.405 40 14.8 2.01 40 10.2 3.20 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. CiHs. cc Abs. CtHiOH. Gms. Caoutchouc, cc. C«H«. cc. Abs. CiHiOHi
0.2 40 18.8 0.2 40 ^21.6
i.o 40 18. 1 I 40 23.3
2 40 17.4 2 ' 40 24.4
SoLUBiLrrv of Caoutchouc in Mixtures of Benzene and Acetone. (Caspari, 19x5.)
Results at 20^. ! Results at 40®. Results at 60^.
Gms. ^^ nju' cc. Gms. __ n.tx^ cc. Gms. -«. r« u cc
Caoutchouc. «• ^-•^^^ (CHi)sC0. Caoutchouc. **• ^^™- (CH,)tCO. Caoutchouc. ^- ^-""^ (CH,)«CO.
O.II
20
iS-7
O.IO
20
19.6
O.IO
20
23
0.80
20
ISO
0.98
20
17.6
1. 01
20
26.4
1.86
20
14.7
CABBAMIDKS.
Solubility in Several Solvents. (Walker and Wood. 1898.)
as Methyl phenvl carbamide (m. pt. 82°), benzyl carbamide (m. pt. 149^).
o tolyl carbamide (m. pt. 185°) and p tolyl carbamide (m. pt. 173®).
Gms. Eadi Carbamide Separately per xoo cc. Sat. Solution.
Solvent. t*. / * ^
05 Methyl Phenyl. Benzyl. ^ Tolyl. 0 Tolyl
Water 45 74 1.71 0.307 0.251
Acetone 23 29.4 3.10 2.66 0.462
Ether 22.5 2.28 0.053 0.062 0.0162
Benzene 44.2 12.4 0.0597 0.043 0.0155
100 gms. chloroform dissolve 0.6-0.7 gm. diiododithio carbamide (CSNsHOiIi
at temp, not stated. (Wener, 191a.)
227 CABBAZOLK
CABBAZOLE (Diphenylene imide) (C«H4)iNH.
loo grams abs. alcohol dissolve 0.92 gm. (CeHOsNH at 14^ and 3.88 gms. at
b. pt.
100 gms. toluene dissolve 0.55 em. (CeHOsNH at 16.5^, and 5.46 gms. at b. pt.
Freezing-point data are given lor mixtures of carbazole and phenanthene by
Garelli (1894).
CABBINOL CHtOH, see Methyl alcohol, p. 435.
Trimethyl CABBINOL (CH,),COH, Triphenyl CABBINOL (C«H8),C0H.
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 4-
bromotoluene are given^by Paterno and Ampola (1897). Results for triphenyl
carbinol + phenol are given by Yamamoto (1908).
CABBON DIOXIDE CO..
Solubility in Water.
(Bohr, 1899; Geffcken, 1904; Just, 190Z.)
Solubffity in Water. ^It^A^^ InijAM
ff. P' I- P. A
o O'SSS 1-713 ••• 1-234 0.678
S 0.277 1.424 ... 1.024 0.577
10 0.231 1. 194 ••• 0.87s 0.503
15 0.197 I. 019 1.070 0.75s 0.443
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 0.530 ... 0.414 0.263
50 0.076 0.436 ... 0.370 0.23s
60 0.058 0.359 ... 0.305 0.183
q — wt. of gas dissolved by 1 00 grams of solvent at a total pressure of 760 mm.
p — the Bunsen Absorption Ooefficient 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 t) '
I « the Ofltwald Solnbility 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. ^ — y* This expression differs from the
Bunsen Absorption Coefficient, fi, 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:
/ - ^ (r + 0.00367 0, /5 « , ■ ^ .,. •
(i + 0.00367 t) .
Solubility in Water at Pressures Above One Atmosphere.
(Wroblewaki — Compt. reod. 94, 1335, '8a.)
jP^^J^. Coefficient of Sftturadon » at: ^^^Mmg Coefficient of Sftturation* at;
o- "-4. pheres. o**- 'a^*-
I 1-797 1.086 20 26.65 17."
S 8.6s S'^S 25 30.55 20.31
10 16.03 9-65 30 33-74 23.25
* Coefficient of absorption is no doubt intended.
CABBON DIOXIDK
228
Solubility op 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 C0|, 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 m compressing COi 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 COi 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 (jb) the volume was
0.102 cc. The volumes of COi used, varied from 60 to 76 cc.
f.
Pianue in
Kg. per
Sq. Cm.
cc. 01 CUi (Keduoed to
I Kg. per Sq. Cm.) Di>-
•olved by I cc. HaO.
f.
Pressure in^
Sq. (^.
Oc. COi (Reduced to z K
per Sq. Cm.) Dissolved
by I cc- HjO.
(«)
(ft)
' (a) "
(A) '
20
25
• • •
1777
60
90
22.74
21.16
{(
30
• • •
1977
u
100
26.22
27.85
ti
40
• • •
21.52
<(
IIO
28.92
28.79
it
50
• ■ •
28.09
«
120
30.20
33.90
n
ss
• • •
29-75
100
60
8.97
• • •
?.5
30
11.77
13 57
tt
70
10. II
6.40
40
14.82
20
tt
80
11.05
9S9
U
so
18.96
24.64
tt
90
12.62
10.85
u
60
22.90
22.50
tt
100
13.63
12.40
tt
70
27.18
27.62
It
IIO
14.88
16.31
u
80
• . •
32.85
tt
120
16.40
15-78
60
40
10.88
9.80
tt
130
17.93
16.89
u
SO
12.24
13 72
tt
140
19.56
17.71
«
60
14.46
15.28
tt
ISO
20.58
17 -49
<(
ro
16.80
17.46
tt
160
22.07
• . •
It
80
19 -74
22.67
tt
170
22.78
• * •
S(x.UBiLiTY OF Carbon Dioxide in Water Expressed in Terms of the Fahr-
enheit Scale of Temperature and Pounds per Square Inch Pressure.
(Heftth, tgis; Anthony, 19x6, see also Riley » 191 1>)
(The
existing data were calculated to
this form,
particularly for
' use
in th
bottling industry.)
Pounds
perSq.
Volumes of CQi Gas Dissolved by One Volume of Water at:
_ A
Inch
pRssure
3t*.
36-.
40'.
44*. 48*.
$5-.
6o*.
6s'.
70-. 7S'.
8o*.
8s*.
90-.
15
346
3.19
2.93
2.70 2(50
2.20
2j02
1.86
I.7I 1.58
1.84
4.35
1.27
20
4.04
3.73
3.42
3.15 2Jp2
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 2.10
1.93
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."
2.86 2.63
342
2.26
2.13
40
6.37
5.89
5.39
4.97 4.61
4.05
3.71
3.42
3.IS 2.89
2.67
2.49
2.34
45
6.9s
6.43
5.88
5-43 5.03
4.43
4.06
3.74
3-44 3.16
2.91
2.72
2.56
50
7.53
6.9s
6.36
5.89 5-45
4.80
4.40
4.0s
3-73 3.42
a. 16
2.94
2.77
55
8.11
7.48
6.86
6.34 5.87
5.17
4.74
4.37
4.02 3.69
3.40
3.17
2.99
60
8.71
8.02
7.35
6.79 6.29
^.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
11.02
10.17
9.31
8.61 7.98
7
6.43
5.92
5.46 5.02
4.62
4.31
4.06
90
12.18
II. 25
10.30
9.52 8.82
7.74
7.II
6.54
6.04 5.55
5-12
4.77
4.49
zoo
13.34
12.33
11.29
10.43 9.66
8.4
7.79
7.18
6.62 6.08
^.60
5.22
4.91
tt
ti
229 CABBON DIOXIDK
Solubility of Cd in Aqueous Solutions of Acids and Salts.
(Ge£fcken.)
Aq. Cms. Acid CO, Dissolved, / at; Aq. Cms. Salt C0> Dissolved. I at;
Solvent. per Liter. x5«. j^*. Solvent per Liter. 15*. 25*.
HQ 18.23 1.043 0.806 CsCl 84.17 1.006 0.781
36.46 1.028 0.799 KCl 37 30 0.976 0.759
72.92 1. 000 0.79s !^C1 7460 0.897 0700
HNOs 31.52 1.078 0.840 KI 83.06 0.992 0.775
63.05 1.086 0.853 ^ 166.12 0.923 0.727
126.10 I. 100 0.877 ^-Br 5955 0.986 0.768
H2SO4 24.52 I. 018 0.794 KBr 119. II 0.914 0.713
49.04 0.978 0.770 KNOg 50.59 1.005 0.784
98.08 0.917 0.730 KNOs 101.19 0.946 0.749
147. 11 0.870 0.698 RbCl 60.47 0.989 0.769
196.15 0.828 0.667 RbCl 120.95 0.921 0.788
Solubility in Aqueous Solutions of Salts. (Mackenzie, 1877.)
Saltm Cms. Salt per Density of Absorption Coefficient a at;
Solution. 100 Cms. Solution. Solution 15*. ' I^
KCl 6.05 1. 021 0.988
8.646 1.053 0.918
11.974 1.080 0.864
22.506 • 1.549 0.688
NaCl 7.062 1.038 0.899(6.4**)
12.995 1.080 0.633 (6. 4**)
17.42 1. 123 0.518(6.4**)
26.00 1.19s 0.347(6.4**)
NH4CI 6.465 1. 021 1.023
«
K
ti
it
tl
ti
tt
tt
it
tt
it
tt
8.723 1.047 I. 000
12.727 1.053 0.922
24.233 1.072 0.813(10**)
ts*.
22-.
0.777
0.670
0.777
0.649
0.720
0.597
0.571
0.480
0.735
• • •
0.557
0.482
0.431
0.389
0.297
0.263
0.825
0.718
0.791
0.702
0.798
0.684
0.738
0.600
.0
8". i6.s'. 22*. 30'
BaCls 7.316 1.068 0.969 0.744 0.680 0.566
9.753 1.092 I. 021 0.645 0.607 0.543
14.030 I. 137 ... 0.618 0.524 0.467
25.215 1.273 0.495 0.618 0.383 0.315
SrCb 9. 51 I 1.087 0.779 0.663 0.581 0.508
12.325 1.1159 0.737 0.586 0.507 0.539
17.713 I. 173 0.606 0.473 0.444 0.367
31.194 1.343 0.285 0.245 0.247 0.223
CaCIa 4.365 1-036 0.942 0.759 0.673 0.596
5.739 1.049 0.855 0.726 0.616 0.527
8.045 1.068 0.838 0.674 0.581 0.500
15-793 1-139 0.632 0.520 0.471 0.400
Data for the solubility of COi in sea water are given by Hamberg (1885).
Aooording to Fox (z9a9a)> analyses of sea water all show an excess of base over add, that is, when OOl
b left out of account. This COi (about 50 cc. per liter) is^f course, in equilibrium with the excess of base,
which is actually equal to about 40 ings. OH per Uter. The partiaJ i^ressure of COi very seldom, if ever,
excecxls 6 in xo.ooo. For the determination of the absorption coefficient of COt there are, consequenthr,
four independent variables to be considered; influence of alkalinity, a chemical influence in addition to the
Enrdy physical influences of temperature, pressure and salinity. For convenience, the dissolved COi may
e considered as made up of two ^rts, about z % dependent upon physical influences alone and a far lar|;er
part dependent upon tJhe 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 (191 7).
tt
tt
tt
it
tt
it
it
It
CARBON DIOXIDE
330
Solubility
OF Carbon Dioxide in Aqueous Solutions of
Salts at 15.2®.
(Setachenow. 1892.)
(Results expressed in terms of cc.
CO, (at
0^ and 760 mm.) dissolved
per I cc
sat. solution.)
Cms.
Db-
Gnn.
Dia-
Cms.
Dia-
Salt.
Salt per
solved
Salt
Salt per
Bolved
Salt
Salt per
aolved
Liter.
C0^
Liter.
C0^
Liter.
.C(V
NHiO
I
1.005
UCl
16.72
1.035
NaCl
12.9
0.978
t<
10
0.985
it
50.15
0.808
II
64
0.760
«
SI. 6
0.941
11
125.4
0.596
tt
128
0.580
(1
172
0.819
II
250.8
0.497
tt
192
0.466
II
258
0.770
u
501 5
0.120
NaBr
115. 1
0.77s
NHiNO*
2.8
1. 013
MgS04
26.5
0.901
II
460.3
0.364
«
II. 2
1.002
11
79. 5
0.669
tt
690.4
0.221
<i
55
0.989
II
159
0.441
NaNO*
89.3
0.835
«
lOI
0.962
u
318
0.188
tt
125
0.762
II
202.1
O.911
KBr
83.9
0.908
tt
208.4
0.621
II
404.3
0.807
tt
167.7
0.819
tt
416.8
0.385
II
810.4
0.612
t€
251-5
0.748
tt
625.2
0.244
(NH4)tS04
72.2
0.712
tt
503.1
0-579
NaClO*
233 -3
0.625
II
144.4
0.575
KI
319-1
0.777
II
349-9
0.506
Ba(NOi)
62.7
0.922
II
478.6
0.688
II
699.8
0.257
Ca(NO»),
41
0.923
II
957.3
0.506
NatS04
14.2
0.950
Citric Add
12
1.007
KSCN
326
0.691
(1
94.8
0.620
II
49
0.975
tt
489
0.590
tt
284.4
0. 234
II
99
0.950
II
978
0.387
ZnS04
38.3
0.903
II
198
0.893
KNO*
58.8
0.959
II
76.7
0.783
II
298
0.841
11
"7.S
0.890
II
230
0.474
it
595
0.719
11
235.1
0.781
II
460
0.209
Several determinations at other temperatures are also given.
Solubility of Carbon Dioxide in Aqueous Salt Solutions at 25*.
(Findlay and Sben, xgxaO
Solubility Gma.
of CO,, Ost. cj. Salt per
wald Ex- ^ xoo cc.
prcssion !». Solution.
0.825 Fe(S04)(NH4)»S04.6HiO 9.51
Salt
Cms.
Salt per
100 cc.
Solution.
dot
Sat.
Sol.
Water alone
NH4CI
j^ Solubility
^'- wald Ex-
pression^.
Sol.
II
«
(I
BaCU
tt
tt
It
Chloral Hy-
drate
2.3s
5.0s
10.02
17.09
2.80
S.81
8.15
9.97
5.08
10.12
1.005 0.791
1. 013 0.754
1.022 0.732
1.045 0.665
I. 018 0.789
1.040
1.054
1.070
1. 019
1. 041
0.741
0.710
0.676
0.815
0.79s
11
II
KCl
II
II
II
Sucrose
II
tt
tt
10.26
22.47
1.84
305
4.58
7.46
2.63
5.16
9.68
12.33
.052
•057
.124
.008
.017
.026
.044
.009
.018
.038
.051
0.641
0.629
0.460
0.792
0.764
0.749
0.701
0.813
0.798
0.767
0.744
Data for KCl 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 Findlav, 1908:
Findlay and Creighton, 1910, iQii; Findlay and Shen, 191 1, 1912; Findlay and
Williams, 1913; Findlay and Howell, 1915.
The solubility of C0| increases slightly with increasing concentrations of
Fe(OH)s, gelatine, silicic acid, aniline (chem. combination occurs), methyl oranee,
blood, serum, peptone, protopeptone, and commercial hemoglobin. The solu-
bility diminishes slightly with increasing concentrations of arsenious sulfide,
dextrine, soluble starch, glycogen (?), ep:g 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 COi 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.
(Christoflf, 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 CO}. The loss of water from the solution
was prevented by first passing the COt through a series of U-tubes containing some
of the same solution. Constant temp, was not employ^ed, 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),S04 I
(NH4)iFc4(S04)4.24H,0 i
KsA]t(S04)4.24H30 I
NH4HBSO4
CUSO4
Lia
MgS04.
COBC of
Aq. Sd.
normal
if
KBr
KQ
KI
KNO»
KsHAs04
KHsAsi04
KH1PO4
KtHPOt
0.25
2
I
o.S
z
2
4
z
z
z
z
O.S
z
z
O.S
«
it
u
«
((
it
<i
a
tt
tt
tt
tt
it
tt
tt
Cms. COi
Absorbed
per 75 cc.
Solvent.
0.1382
O.Z093
O.099Z
O.ZOS4
0.7672
0.07SZ
0.Z087
0.Z209
o . Z020
0.0662
0.0527
0.1280
O.Z2Z3
O.Z204
0.Z23Z
o.zzzo
0.0813
0.0860
o.49oo(?)
Salt in Aq.
Solution.
K4P4Q11
KHSO4
KjS04
tt
tt
tt
tt
It
NaBQs
NaCl
Na,P04.z2H,0
Na4PiOr.zoHiO
Na4P40i,
ZnS04
Sugar
tt
tt
Cone, of
Aq. Sol.
z normal
it
tt
tt
0.66
2.
0.66
z
0.025
0.Z25
0.25
sat. sol.
" 4-crysts.
0.25 normal
z
tt
tt
tt
I
I
1
2
o.z
O.S
z
(I
tt
tl
«
tt
tt
Cms. CX)i
Absorbed
per 75 oc
Solvent.
O.Z237
0.Z020
o.zooo
o.zr40
0.Z002
0.2205
0.5317
0.85ZZ
Z.8285
3.2240
0.8Z22
O.ZO5O
0.5828
0.8463
0.0700
0.0720
O.Z225
O.ZO89
O.O93Z
Solubility op Carbon Dioxide in Aqueous Solutions of Sulfuric Acid.
Results at 15.5^. (Christoff, 1905.)
Percent
, H«S04
in Solvent.
2-5
5
10
20
30
Cms. COi
Absoriwd per
75 cc. Solvent.
0.1282
o . 1079
0.0833
0 07SS
0.0751
Percent
H,S0,
in Solvent.
40
45
70
90
Cms. C0|
Absorbed per
75 cc. Solvent
0.0713
0.0725
0.0918
0.1433
Results at 20®. (ChriatofF, 1906.)
Per cent Solubility of C0|,
HtSOf Ostwald Expres-
in Solvent. sion ^.
o 0.9674
35.82 0.6521
61.62 O.719I
95.6 0.9924
96 P = 0.926 (Bohr.igio.)
Solubility of Carbon Dioxide in Aqueous Solutions of Chloral Hydrate
AND OF Glycerol at 15®.
Results in terms of the Bunsen absorption coefficient fi, and also the Ostwald
(von Hanunel, 19x5.)
solubility expression / (see p. 227).
In Aq. Chloral Hydrate.
CCU.CH(OH)j per ^\ ^^^^
100 Cms. Aq. Sot
17.7
31 -6
38.3
49.8
S7I
68.8
79-4
0u-
0.885
0.803
0.781
0.760
0.765
0.797
0.903
SolubiUty,
0.93s
0.848
0.825
0.802
0.808
0.842
0.9S3
Cms.
In Aq. Gljrcerol.
(CHt0H)sCH0H per
100 Gms. Aq. Sol.
O
26.11
43-72
62.14
77.7s
90.74
99.26
Abs. Coef.,
1.008
0.78s
0.639
O.51I
0.430
0.404
0.410
SolubOity,
hi'
1.064
0.829
0.675
0.540
0.4S4
0.427
0.438
CARBON DlOZmS
333
— 20
— 10
o
+ 10
20
as
30
40
45
Density of
AloohoL
0.998
0.969
0.960(22.4**)
0.956
0.93s (17**)
Solubility of Carbon Dioxide in Alcohol.
(Bohr — Wied. Ann. Physik.U] x. 247. '00)
In 99 per cent Alcohol. In 98.7 per cent Alcohol.
oc COi (at o^ and 760 mm.) per i cc. cc. COi (at o^ and 760 mm.) per i oc
Alcohol. Sat. Solution.
Alcohol. Sat. Solution.'
38.41
7SI
S-7S
4-44
3S7
2.98
2.76
aS7
2.20
2.01
35-93
7.41
5-69
4.40
3SS
2.96
2.74
2.56
2.19
2.00
39 89
7-25
S-43
435
37.22
7.16
S-38
4-31
. . •
• • •
• • •
• • •
• • •
• • •
Solubilitt in Aqueous Alcohol at 2o^
(Mttller, 1889; Lubarsch, 1889.)
Percent Abs. C^f.
Alcohol by Wt. ofCOt.a.
1.07
Density of
Alcoh(ri.
22.76
28.46
31.17
42. IS
0.861
0.841
0.792
0.801
0.877
0.922
0.870(18.8**)
0.83s (16")
0.795(19'')
Percent
Alcohol by Wt.
49 o
71. 1
85.3
99-7
Abs. Coef.
of COiya.
0.982
1.293
1-974
2.719
Solubility in Aqueous Alcohol at 25*.
(Findlay and Shen, 191 1.)
Results for alcohol,
of J|| = 0.9931
(2.95 gms. per 100 cc.).
Solubility of COk.
Ostwald Expres-
sion^.
Results for alcohol,
of d^ » 0.9929
(3.01 gms. per 100 cc.).
Results for alcohol,
of J}| = 0.9834
(8.83 gms. per 100 oc.).
Pressure
m.pi. Hig.
737
836
1073
1338
0.812
0.813
0.811
0.811
Pressure
in.ni. Hg.
745
937
1083
1357
Solubility of (X)i,
Ostwald Expres-
sion^.
0.814
0.815
0.813
0.812
Pressure
ni.ni. Hg.
747
942
i(^
1360
SolubUity of COi.
Ostwald Expres-
sion In.
0.786
0.784
0.785
0.788
These authors also showed that the solubility of COi in wort containing 13 gms.
solids per 100 cc. is less than in water; also that the solubility of CO} 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 fi, see p. 227. (Usher, 19x0.)
Aqueous Solu-
tion of:
Gm.
Mols. per
later.
Sol.
Absorp*
tion
Coef. fi.
Aqueous Solu-
tion of :
Gm.
Mols. per
Liter.
dn of Aq.
Sol.
Absorp-
tion
Coef.^.
Water Alone
• • •
• • •
0.877
Resordnol
O.S
1.0096
0.901
Sucrose
O.I2S
1.0152
0.846
Catechol
OS
1. 0107
0.868
tt
0.25
I. 0313
0.815
Urethan
o.S
1.0037
0.869
it
0.50
1.0637
0.756
Carbamide
0.5
1.0072
0.864
it
I
I.1281
0.649
Thiocarbamide
o.S
1.0092
0.859
Dextrose
0.5
1.0328
0.792
Antipyrine
o.S
I. 0134
0.859
Mannitol
O.S
1.0303
0.782
Acetamide
OS
1.0005
0.879
Glycine
o-S
I.OI41
0.843
Acetic Acid
o.S
1.0026
0.868
Pyrogallol
o.S
I. 0172
0.853
n Propyl Alcohol
o.S
0.9939
0.869
Quinol
o.S
1009s
0.887
233 CARBON DIOZXDI
Solubility of Carbon Dioxide in Organic Solvents at Low Tbm-
PERATURBS AND PRESSURES. (Stem, 191 1-13.)
Very accurate determinations with an elaborate apparatus. The results are
expreraed in terms of K* » the number of cc. of COi, 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 liauid.
Therefore Bunsen coef . fi » K'd. The results are also expressed in terms ot the
Ostwald solubility expression / (see p. 227).
Solvent, CiHtOH. Solvent,
CH«0H.
Solvent.
(CH,)iCO.
Solvent.
CH«CUk.CtH».
Solvent,
CHiCOiCHt.
Preasitre
° t*. in nun.
d-mu — 0.87a.
^.
0.884.
d-m^ * 0.900
^^-1.0x7.
rf-t«*»'0-s6.
Hg.
dL«^ * 0.856.
^.
0.866.
rf-|ji- 0.879.
dL|j|- 0.994
d-mm^ 1.032.
K\ I.
' K\
/.
K\ /.
K', I.
' K\ L '
-78 SO
107
194
120.5
311 196.6
250.2 177.5
304.9 224.1
" 100
III.8 68.4
19s
1 19.6
322 198.I
255.6 177.I
315 224.3
" 200
iiS-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
Z22.2
400 208.8
310.9 183.2
389.3 225.6
" 700
138.6 74.7
260
126.8
545.5 . . •
• • • ■ • •
• • • ■ • •
-59 100
40.85 27.27
63
42.S
97.8 67.2
85.3 65.6
94.3 75.8
" 200
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
43-1
106.6 72.8
9Z.6 66.7
103.6 77.6
" 700
44.15 28.10
69
43.35
Z18.8 72.8
IOI.5 69.7
II 2.9 79
S(x.uBiLrrT OF Carbon Dioxide in Organic Solvents at High Pressures.
(See Note. p. 228.) ^Sander, 1911-ia.)
Pies- Cc. of COi (Reduced to i Kg per Sq. Cm.) Dissolved at the Temp, and Pressure of Experi-
soxe in ment by x cc. of Sat. Solution in:
perSq.CSHiOH
OHtOH
(CtH«)tO CHiCOOCtHi OHt
CtHsCl
CtHtRr
CANOi
CACHi
Cm.
(0.093 cc,
1 (0.103 cc.) (0.13X cc.)
(0.Z55 cc.) (0.08 cc.) (0.106 cc
) (0.X13 cc]
1 (0.X64 cc)
(0.1Z4CC.)
Results at 20®.
20
• • •
56.16
■ • «
71.16
62.61
50.83
57-12
57.91
30
ZO4.8
86.62
• • •
188.2 125.3
95.22
82.29
92.50
XO3.3
40
149.7
I22.I
• • •
227.9 192.4
137.3
I2I.I
"5-9
155.9
50
188.8
174.6
• • •
264.3
Results at 35*".
187.5
160
155-9
235.8
20
• • •
40
• • •
48.65
46.66
43.38
44.48
49.6
40
I13.I
98.16
• • •
188.4 138.3
XOI.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
• • •
■ • • • • •
Results at eo"".
• • •
233.9
227
• « ■
20
« ■ •
24.73
« • •
34.57
35.86
30.58
31.38
• • •
40
72.82
64.65
* ft •
140.5 88.71
7369
62.64
52.26
78.67
60
122.5
111.5
195.4
186.7 156.6
I18.I
98.73
72.15
1 28. 1
80
167.9
159.2
221.4
223.4 215
149.3
13 1. 4
85.03
171.9
100
195.7
213-9
248.7
284.4
Results at 100**.
• • •
169.7
• • •
210
30
• • •
• • •
• ■ •
• • • • • •
3365
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
lOZ
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
II 7.6
100
145.7
144.7
175.4
191.5 212.9
121.5
118
• • •
149
120
174.6
175.4
• ■ ■
258.2
140.7
140.7
• • •
X71.8
130
182.6
* ...
• ■ •
• • m • • •
146.8
V • •
• • •
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 COj varied from about 55 to 77 cc. in the several
cases. The increasing content of COt 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 ol the applicability of Henry's Law in the
present case, are given.
CARBON DIOXIDE
234
Solubility of Carbon Dioxidb in Organic Scx^vents.
(Just. 1901.)
The determinations are described in ^eat detail. Results are given in terms
of the Ostwald solubility expression / (see p. 227).
Solvent.
Water
Glycerol
Carbon Disulfide
lodobenzene
Aniline
0 Toluidine
i(
Eugenol
Benzene- Trichloride
Cumol
Carven
Dichlorhydrine
Amyl Alcohol
Bromobenzene
Isobutyl Alcohol
Benzyfchloride
Metoxylol
Ethylenebromide
Chlorobenzene
Carbontetrachloride
Propylenebromide
Toluene
Im.
^
Ai.
0.8256
• • ■
• • «
0.0302
• ■ •
• • •
0.8699
0.8888
0.9446
1. 301
1.371
1.440
1.324
1.434
1.531
I.381
1.473
1-539
1.436
1.581
1.730
1.539
1.653
Z.762
1.643
■ ■ •
• ■ •
1.782
1.879
1.978
1.802
1.92 1
2.030
1. 8 10
1.917
2.034
1.831
1. 941
2.058
1.842
1.964
2.092
1.849
1.964
2.088
1.938
2.072
2.180
2.090
2.216
2.346
2.IS7
2.294
2.424
2.265
2.420
2.581
2.294
2.502
2.603
2.301
2.453
2.586
2.305
2.426
2.557
Solvent.
Benzene
Amylbromide
Nitrobenzene
Propyl Alcohol
Carvol
Ethyl Alcohol (97%)
Benzaldehyde
Amylchloride
Isobutylchloride
Chloroform
Butyric Add
Ethylene Chloride
Pyridine
Methyl Alcohol
Amylformate
Propionic Acid
Amyl Acetate
Acetic Add (glacial)
Isobutyl Acetate
Acetic Anhydride
Acetone <
Methyl Acetate
1m.
w
lu.
2.42s
2.540
2.710
2.455
2.638
2.803
2.456
2.655
2.845
2.498
• ■ •
• ■ •
2.498
2.690
2.914
2.706
2.923
3.130
2.84Z
3.057
3.304
2.910
3.127
3.363
3.105
3.388
3.659
3.430
3.681
3.956
3.478
3.767
4.084
3.525
3-795
4.061
3.656
3.862
4.291
3.837
4.205
4.606
4.026
4.329
4.646
4.078
4.407
4.787
4. 1 19
4.4"
4.850
4.679
5.129
5.614
4.691
4.968
■ • •
5.206
5.720
6.218
6.295
6.921
• • •
6.494
. . •
• • •
Solubility op Carbon Dioxide in Ethyl Ether. V Results in Terms of the
^^ Ostwald Solubility Expression /.
^ = 7-330.
(Christoflf, 19x2.)
do = 6.044.
5.465.
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 CO} 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 /9 of COs 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 COt by rubber and carbon are given by Reychler
(1910).
Data for the absorption of CO} by hemoglobin are given by Jolin (1889).
Data for the distribution of CO2 between air and HsO, air and aq. HsSOi and
air and toluene at various temperatures, are given by Hantzsch and Vagt (1901).
Data for the freezing-points of mixtures of CO} and methyl-ether and for COt
and methyl alcohol are given by Baume and Perrot (191 1» 1914).
235
CARBON DISUUrXDI
CARBON DISULTIDB CS|.
SoLUBiLrrT IN Water.
(Chaood and Paimentkr, 1885; Rex, 1906.)
f.
O
5
10
IS
20
2S
Gnms CSipec xoo
cc
[Solution.
0.204
0.199
0.194
0.187
0.179
0.169
Gms.HiO
0.258
. . •
0.239
...
0.317
30
35
40
45
49
Gtains CStpflsrioo
cc
SduUon.
o.iSS
0.137
O.III
0.070
0.014
Gma. HiO
(Rex).
0-I9S
^100 cc. H]0 dissolve 0.174 cc CSi at 22^; Vol. of solutioa » ioo.2o8» Sp. Gr. »
0.9981.
100 cc. CSi dissolve 0.961 cc. HiO at 22®; Vol. of solutioa -
1.253.
Solubility of Carbon Disulfidb in:
Aq. Solutions of Ethyl Alcohol at 17"".
(Tucfaschmidt and FoUeuins, 1871.)
100.961 » Sp. Gr. «»
(Hen. 1898^
Methyl Alcohol.
(Rothxnimd. 1898.)
Wt percent
Alcohol.
100
98-5
98.15
96.95 .
93 54
c&CSt
per loooc
Solvent.
00
182
132
100
70
Wt. per cent ^,^,
Alcohol.
91 -37
84.12
76.02
48.40
47 90
per xoocc.
Solvent.
SO
30
20
2
o
f.
10
20
2S
30
35
wt per CSi in:
CH«OH
Layer.
451
SO. 8
54.2
58.4
64
40.5 (crit. temp.) 80.5
SOLUBILITT OF CaRBON DiSULFIDB IN EtHYL AlCOHOL. (Gtltfalie, 1884^
CSi
Layer.
983
97.2
96.4
9SS
93 S
Cms. CSi per xoo
Cms. CSt+CsHriOH.
94-94
89.54
84.89
79.96
65.11
59.58
29.92
An)earance on Cooling in Ice and
Salt Mixture.
Remains dear down to —18.4
Becomes turbid at —14.4
-15.9
— 16. 1
tt
tl
II
u
t(
tl
tt
-17.7
Remains clear down to —20
((
tt
tt
tt
tt
CARBON MONOXIDE CO.
SCH.UBILITY IN Watbr.
/^."Solu.. „ 4.
biUty." *• ^'
0.03516 0.0044 40
0.03122 0.0039 50
0.02782 0.0035 60
0.02501 0.0031 70
0.02266 0.0028 80
0.02076 0.0026 90
O.OI915 0.0024 100
O
5
10
15
20
25
30
0, "Absorp.
. Cod."
0.03537
0.03149
0.02816
0.02543
0.02319
0.02142
0.01998
(WinUer.'igox.)
0» "Ahaorp,
Coef."
0.0177s
O.O1615
0.01488
0.01440
0.01430
0.01420
O.OI410
0' "Solu-
biUty."
0.01647
0.01420
O.OII97
0.00998
0.00762
0.00438
0.00000
f-
0.0021
0.0018
0.0015
0.0013
O.OOIO
0.0006
0.0000
$ » vol. of CO absorbed by i volume of the liquid at a partial pressure of 760
mm. See p. 227.
fi^ = vol. of CO (reduced to o® and 760 mm.) absorbed by I volume of the liquid
under a total pressure of 760 mm.
q a grams of CO dissolved by 100 grams H2O 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.
327), was found by Findiay and Creighton (191 1) to be /u » 0.0154.
Data for the solubility of CO in water at high pressures are given by Cassuto,
1913.
Data for the solubility of CO in aq. NaOH solutions are given by Fonda, 19 10.
Results for the solubility of CO in aq. HsS04 at 20^ are given in terms of the
Ostwald solubility expression / by Christoff (1906) as follows:
lu for HjO « 0.02482, la for 35.82% HjSOi = 0.0114, In for 61.62% HtSOi =
0.00958, In for 95.6% HjSOi «= 0.02327 and 0.02164.
Data for the solubility of CO in ox blood and ox serum at 25^ are given by
Findiay 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 mixtiune)
occurred in three hours.
Data for the solubility of CO in aqueous hemoglobin solutions are given by
Hafner (1895) and HUfner and Kulz (1895).
Solubility of Carbon Monoxide in Aqueous Alcohol S(X.utions
at 20^ and 760 mm. pressure.
(Labaiscfa,
1889.)
AkohoL
Vol. %
Absorbed CO.
AloohoL
AbaorbiBdCO.
0
2.41
28.57
I SO
9.09
16.67
23.08
1.87
1.7s
1.68
33-33
SO
1.94
3-20
Solubility of Carbon Monoxide in Organic Solvents.
(Just, 1901.)
Results in terms of the Ostwald Solubility Expression, see p. 227.
Solvent. /«. in. Solvent.
Water 0.02404 0.02586 Toluene
Aniline o 05358 0.0S055 Ethyl Alcohol
Carbon Disulfide 0.08314 0.081 12 Chloroform
Nitrobenzene 0.09366 0.09105 Methyl Alcohol
Benzene 0.1707 0.1645 Amyl Acetate
Acetic Add 0.17 14 0.1689 Acetone
Amyl Alcohol o . 1 7 14 o . 1 706 Isobutyl Acetate
Xylene 0.1781 0.1744 Ethyl Acetate
100 volumes of petroleum absorb 12.3 vols. CO at 20^ and 13.4 vols, at I0^
(Gniewott and Walfiai, 1887^
Solubility of Carbon Monoxide in Ethyl Ether.
(Christoff, 191a.)
Results in terms of the Ostwald solubility expression, see p. 227.
A) «= 0.3618. /lo = 0.3842.
Is.
l»
0.1808
0.Z742
O.I92I
0.I90I
0.1954
0.1897
0.195s
0.1830
0.2140
0.2108
0.2225
0.2128
0.2365
0.2314
0.2516
0.2419
237
CARBON MONOXIDE
Solubility of Carbon Monoxide in Mixtures of Acetic Acid
Other Solvents at 25^.
(Skirrow, 1902.)
Results in terms of the Ostwald solubility expression, see p. 227.
AND
Mixture of
Acetic Ac
CHKX)OH
CO.
Im.
Mixture of
Acetic Ac
cacbdn
^-
and:
in Mixture.
and:
in Mixture.
Aniline
100
0.173
Chloroform
56-4
0.196
it
86. s
O.IIO
u
0
0.206
it
58.3
0.070
Nitrobenzene
78.4
0.156
tt
17.8
0.058
«
49
0.130
tt
0
0-053
u
0
0.093
Benzene
67.5
0.199
Toluene
74.7
O.I9I
u
335
0.198
K
56.9
0.19s
tt
19.2
0.190
tt
20.5
0.190
ti
0
0.174
tt
0
0.182
SOLTTBlLnY OF CaRBON MoNOXIDB IN MIXTURES OF ACETONB AND
Other Solvents at 25^.
(Skixiow.)
Mixtore of Acetone
and:
%«:to«co
In Mixture.
ByWt.
CO.
Mixture of Acetone
and:
inMurture.
ByWt.
CO.
Im.
Aniline
100
0.238
Chloroform
66.6
0.226
tt
79.2
0.179
tt
26.5
0.212
tt
44.9
O.IIO
tt
0
0.207
tt
0
0.053
P Naphthol
86
0.190
Carbon Disulfide 82
0.236
731
0.169
tt
50.5
0.227
Nitrobenzene
78.4
0.207
it
26
0.187
tt
46.8
0.157
tt
14.5
0.144
it
0
0.093
tt
0
0.096
Phenanthrene
87.2
0.205
Naphthalene
86.7
0.199
((
75
0.183
tt
72.6
0.187
Solubility
OF Carbon Monoxide in Mixtures of Benzene
Other Solvents at 25®.
(Skinow, igoa.V
AND
The solubility of the CO given in terms of the Ostwald expression, see p. 227.
Mixture of Bcmene
and:
Naphthalene
it
tt
Phenanthrene
it
a Naphthol
it
fi Naphthol
tt
%C«H.in
Mixture.
ByWt.
100
88.5
66.2
89.5
72.6
96.5
87.9
97-9
95-6
CO.
Im,
0.174
0.164
O.I4I
0.144
0.127
0.149
0.139
0.158
0.149
Mixture of Benaene
and:
Aniline
tt
tt
tt
it
Nitrobenzene
a
it
Ethyl Alconol
%CtHiin
Mixture.
ByWt.
87.3
71.7
42.6
21.2
O
71.8
45. 1
o
47.7
o
CO.
^.
0.156
0.I3I
0.09s
0.068
O.OS3
0.152
0.127
0.093
0.181
0.192
CARBON MONOXIDE
238
Solubility of Carbon Monoxide in Mixtukbs of Tolubnb amd
Othbr Solvbnts at 25^
(Skinow, 1903.)
Aniline
«
Mixture <A Tot CtHtCH» in Mixture. cO.
ueneuid: Wt. %. Mol. %. hh
ZOO xoo 0.183
93-4 935 0.169
80.1 80.3 0.148
55.4 55-6 o.iis
25.4 25.6 0.077
o o 0.053
Naphthalene 92.9 94.8 0.169
84.9 88.7 0.161
77.3 82.5 O.IS3
Mixture of To&- CiH>CHt in Mixture, qq.
it
«
tt
ueneand:
a Naphthol
Nitzobenzene
Phenanthrene
II
wt.%.
955
91.2
81.7
50.8
33. 7
o
94.4
88.8
78.4
Mol.%.
97.1
94.2
85.7
58.1
29.3
o
97
93-9
87. S
O.171
0.162
0.160
0.131
O.Z08
0.093
0.170
O.161
0.147
Solubility of Carbon Monoxide in' Mixtures of Organic Solvents at 25^
(Skinow.)
Chloroform and Methyl Alcohol
ti tt
% of Latter in Mixture.
C(
it
Carbon Bisulphide and Ethyl Di Chloride
ByWt.
00
13 o
100
ByMoL
u
it
ti
tt
tt
ti
it
u
Methyl Alcohol and Glycerine
it
tt
M
tt
tt
ti
ii
tt
0.0
39-6
60.5
77.1
100. o
100
75
SI
18.4
0.0
0.0
301
50.1
68.9
100. o
CO
0.307
0.302
0.196
0.147
O.IS7
0.160
0.140
0.083
0.196
0.096
0.052
0.025
very small
Note. — Prom the results shown in the preceding five tables, it is
concluded that the solubility of carbon monoxide in various mixttires
of organic solvents is, in general, an additive fimction.
OABBON OZTSUUIDE COS.
Solubility of Carbon Oxtsulftob in Water.
(Winkler, 1906.)
t*. fi, q. t*. fi. q.
o 1-333 o-3S^ 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 0 and q see Carbon Dioxide, p. 227.
S(x.UBiLiTY OF Carbon OxYsuLFmE in Several Solvents.
Water
Solvent. t*.
13s
20
Alcohol 22
Toluene 22
HCl solution of CuCl 13 . 5
I gm. KOH+ 2CC.HiO+ 2CC.CjH60H 13 . 5
Pyridine
Nitrobenzene
cc cos per
100 oc. Solvent.
Authocity.
80
(Hempd, 1901.)
54
(Stock and Kint zgtrO
800
M «
1500
M «
20
(Hempd, 190ZO
7200
M
44'
«
12.0
11
239 CARBON TITRACHLOBIDI
GABBON TBTBAGHLOBIDB CCU.
SCX^UBIUTT IN WaTSS. (Rex, 1906.)
r. or. !©• «©• 30*
Gms. CCI4 per icx> gms. HsO 0.097 0.083 0.080 0.085
Rbcifrgcal S(X.ubility of Carbon Tbtkachloridb, Alcohol and Water.
(Curtis and Titus. 19x5.)
Alcohol was added from a weight buret to mixtures of weighed amounts of
ecu and H^, stirred vigorously at I9.75^ untU the mixture became homogeneous.
Per oeot
Percent
Percent
CCk.
CiHiOH.
EW).
41.94
4319
14.89
33 07
47.68
19.25
25.46
SO SO
24.04
17.00
SI-9S
31.05
14.02
S^S^
34.42
10 53
S0.97
38.50
In Older to determine 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.
»^r,H.oH-»-*^
... . ecu - «. . " CCU
B *• ecu
B z.o9ia.
Percent
CritSoL
Percent
Ciit Sol. Per cent
Crit. Sol.
Percent
Crit-SoL
EW).
f.
£M).
f. BM).
f.
CtHiOH.
f.
24.25
-1.8
12.47
2.03 6.84
12.7
47.43
44. 5
24.61
+3.6
13.9s
23.9 7.16
21.5s
47.83
395
25.13
10.6
14.45
29.8 7.3s
27.2
48.6
30.6'
25.64
17
14.85
35.4 7.54
31-3
49.61
19.9
26.14
24. S
15.3
3955 7.84
36.8
50.07
14.6
27.15
31.45^
35. 5(?)
15.67
42.75 8.02
39.75
50.50
9. IS
28.52
16.02
455 8.28
44.1
SI. 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+Cl are given by Waentig and Mcintosh (19 16).
CABMIME.
100 gms. HiO dissolve 0.13 gm. carmine at 20-25^ (Dehn» 1917.)
*^ pyridine " 3.34 gms. " " "
50% aq. pyridine " 2.03 " " " "
CABVACBOL (CH,),CH.CH,(CH,)OH.
MisciBiLiTY OF Aq. Alkaline Solutions op Carvacrol with Several
Organic Compounds Insoluble in Water. (Sbeubie, 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 occiured. Temperature not stated.
(Composition of Homogeneous Solutions.
Aq. KOH. Aq. Inaol. (Compd. Csrvacrol.
5 CC. 2 CC. r= 1.64 gms.) Octyl(i) Alcohol i .8 gms.
5" 5CC. (~4.i 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 "
(s).» tlw BQCinal Moaodaiy octyl alcohol, U., the so<aIled capcyl alcohol, CHi((34)i.CH(0q)CHa.
CABVOZIMB
240
CABVOZIMB C]oH4:NOH djandi.
SoLVBiLnY IN Aqueous Alcohol of dn^ - 0.9125 (51.6 Pbk Cent
CiHiOH).. (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 carvoximei in addition to the curves for
dextro and inactive carvoxime. The curves for these latter intersect the curve
for liquid carvoxime respectively at 5 1. 7", the m. pt. of dextro, and 70.5" the m.pt.
of inactive carvoxime.
GlIM.
Solvent, pel
Mols. Carvoxime
' 100 Cms. Solvent.
t* of Solution.
Solid Phase.
Carvoziiiie.
SdM.
liquid.
0.0668
1.0868
0.0373
384
13 -9
d Carvoxime
0.1232
1.0830
0.0689
45-8
319
u
0.2026
I. 0218
0.1202
50-3
49-8
It
0.4040
I. 0218
0.2396
• • •
79.6
it
0.4128
0.8130
0.3077
• • •
945
u
0.0657
1.0980
0.0363
54.2
• • •
i Carvoxime
O.I2I2
I.O161
0.0723
62. s
33-7
c<
0.2715
I. 0129
0.1625
69.25
61.3
u
0.37SS
1.0384
0.2192
• • •
76.6
it
0.4496
0.7768
0.3409
• • •
102.9
tt
Solubility in
d LnCONBNB.
(Goldachmidt and Cooper, i
898.)
Gntt. CiJIt:N0H
Cms. CioHi:NOH
t*. per 100
Gins.
Solid Phase.
f.
per 100 Cms.
Solid PhaM.
dLiznonene.
d Lixnonene.
24.6
44
.6 I Carvoxiine
48
198.7
/ Carvoxime
30
59
.2 I
49-4
199.7
d
30.3
63
•3 d
ss-^
325- 1
I
384
104.3 /
SS-9
346.6
d
39-3
103
.1 d
S8.8
560
d
431
130
.8 /
63.2
1269.3
d
Freezinff-point data are given for mixtures of d and / carvoxime by Adriani,
1900 and by Beck, 1904.
CASKm.
100 gms. HsO dissolve 2.01 gms. casein at 20-25^. (Defan. 19x7.)
100 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)t at various temperatures, are given
by Robertson, 1908.
CATECHOL oC6H4(OH),.
Freezing-point data (solubilities, see footnote, p. i) are given for mixtures of
catechol and picric add, catechol and a naphthylamine and catechol and p tolui-
dine by Philip and Smith, 1905.
CEPHABLINE Salts.
Solubility in Water. (Caxr and Pyman, 1914.)
Cephadine Hydrochloride C28lW)4N2.2HC1.7H|0 17-18 26.5
acid " C»Hjrt04N,.sHCl 18 about 50
Hydrobromide CttHs^4N>.2HBr.7H^ 17-18 5.4(driedatioo-)
«
it
241
CEBTOM ACETATB
OERIUM AOETATE, BUTTBATE, FORMATE, etc.
Sdt.
Acetate
Butyrate
Iso Butyrate
Fonnate
Propionate
Solubility in Water.
(Wolff — Z. anorg. Chem. 45. xos. '05.)
Grams Anhydrooa Salt per xoo Gms. Solution al3
Fonnuhu
Ce(CA0,),.ilH20
Ce(C*HrOJ„and3H,0
Ce(QIIrOJ,.3H,0
Ce(CHOa),
CeCQiHjO JrHjO, and 3H,0
ir
3-544
• • •
15 •
19.61
3406
6.603(20.4**)
0.398(13^)
18.99
76'.
12.97
1.984
3.39
o-374(75-3T
15-93
OEBIUM AMMONIUM NITRATE (Ceri) Ce(NO«)4.2NH4NOa.
Solubility in Water.
(Wolff.)
25
35-2
45-3
64 S
85.6
Gms. per 100 Gms.
Solution.
NH«.
4-065
4-273
4.489
4.625
4-778
6. 117
Co,
15-1^
16. IC
16. 6g
(17.40 Ce
(IS-'
[5 .03 Ce IV
(18.16 Ce
(15.79 Ce IV
22.82 Ce
22CeIV
\*j -
i22.
l6.
Atomic
Relation.
Gms. (XN08)4.9NH4NOt
per 100 Gms.
NH«
2.08
2.06
2.08
2.06
2-39
2.04
2. 34
a. 08
2.95
Ce.
Ce
CelV
Ce
Ce IV
Ce
CelV
Solution.
58-49
61.79
64.51
66.84
69.40
88.03
Water.
140.9
161. 7
174.9
201.6
226.8
735-4
CERIUM AMMONIUM NITRATE (Cero) Ce(N0,),.2Na4l^0,.4HA
Solubility in Water.
(Wolff.)
Gms.
^
xoo Gms.
iution.
Atomic Relaticui.
8.75
£•5.0
45 -o
6o-o
65.06
NH4.
4.787
509
5 53
6.01
6. II
Ce.
18.56
19.80
21 .06
22.77
23.42
NH4
1.999
1-995
2.037
2-054
2.022
Gms. Ce(N0ih|.2NH«N0»
per zoo Gms.
^' Solution. Water.
70.2
74-8
80.4
87.2
89.1
23s S
296.8
410.2
681. a
817.4
OERIUM AMMONIUM SULPHATE Cea(S04),.(NHJ,S04.8H,0.
Solubility in Water.
(Wolff.)
Gms.
Cea(S04)».(NH«),S0«
per loq Gms.
Solution! Water'.
22
35
'3
.1
45-2
5.06
4-93
4.76
S-33
5.18
4.99
SoUd
Phase.
.8H,0
Gms.
Ces(S04)».(NH*),S0«
per 100 Gms.
Solution. Water.
SoUd
Phase.
45 o
55-25
75-4
85.2
2.91
2.16
1.46
1. 17
2-99
2.21
1.48
1. 18
Anhydride
((
((
ti
GEB0U8 CHLORIDE 242
CEB0X7S CHLORIDE CeCb.
100 oc. anhydrous hydrazine dissolve 3 gms. CeCU, with evolution of ga8» at
room temp. (Welsh and Biodenon, 1915.)
CERIUM CITRATE 2(CeC«Hf07).7HsO.
100 gms. of aq. citric acid solution containing 10 gms. citric add per 100 cc.,
dissolve 0.3 gm. CeCCeHjO) at 20**. (Holmbos, 1907.)
CTRIUM COBALTICYANIDE Cet(CoC«N6)2.9HA
100 gms. aq. 10% HCl (dvt - 1.05) dissolve 1.075 gms. of the salt at 25^.
CJames and WiUand, 1916.)
CERIUM FLUORIDE CeF,.
Freezing-point lowering data are given for mixtures of CeFt + KF by Puschin
and Baskow, 1913.
CERIUM GLYCOLATE Ce(CsHA),.
i One liter H2O dissolves 3.563 gms. of thesalt at 20^ Qantsch and Gnmkniut, Z9i»-Z5.)
CERIUM lODATE Ce(IOs),.
One liter sat. aqueous solution contains i .456 gms.Ce (IOi)s, determined by a chem-
ical method, and 1.636 gms. determined electrolytically. (Rimbacfa and Schubert, 1909.)
CERIUM MALONATE CeiCC.HsOOs + 6HsO.
Solvent f ^"*- Cei(C«HiO0i per
^'^*^** *• 100 Gnuns. Solvent.
Aq. Ammonium Malonate, containing 10 gms. per 100 cc. 20 0.2
Aq. Malonic Add, containing 20 gms. per 100 cc. 20 0.6
(Hdmbeig, 1907.)
CERIUM Magnesium, etc., NITRATES.
Solubility in Cong. Aq. HNOi (iy = i .325 = 51 .59'Gms. HNOi per 100 cc.) at i6*.
G&ntBch, 19x2.)
Cerimn magnesiimi nitrate, i liter sat. solution contains 58.5 gms. [Ce(N0ft)«]Mgt. 24H«0.
" nickel " " " " 75.3 " " Ni, "
" cobalt '* " " " 103.3 " " Co, "
" 2dnc " " " " 111.7 " " Zn, "
" manganese " " " " 178.8 " " Mn, "
CERIUM OXALATE Cei(C204),.9HA
One liter HsO dissolves 0.00041 gm. CeiCCsOOs at 35^, determined by the elec*
trolytic method. (Rimbach and Schubert, 1909.)
SCX^UBILITY OF CeRIUM OXALATE IN AqUEOUS SOLUTIONS OF SULFUKIC
Acid and of Oxalic Acid at 25®.
(Hauaer and Wirth, 1908; Wirth, 19x2.)
Cone of Gms. per 100 Gms. _ ... Gms. per 100 Gms. _ ,. .
Aoueous Sat..Sol. ^ Cone of Aq. Acid. ^.Soi. ^
Acid. CcOi« Ce,(CiOi)j. CeO,- Ce«(CiO«)«:
o. Ill HsS04 0.0136 0.0215 Ce(C^4)s-9H|0o.in(C00H)s 0.0020 o.oo32Cei(C^«)s.9B^
0.5 " 0.0524 0.0828 " 0.5 " 0.0083 0.0131
X.O " 0.1 14 0.1802 " 1.0 " 0.0040 0.0063
1445 " 0.1764 0.2788 •* 3-2 " (sat.) 0.0019 0.0030
2.39 " 0.3083 0.4871 " 0.05 " +.osnHjS040.oo30 0.0047 "
2.9 " 0.4724 0.7467 •* 0.05 " -h-S " 0.0025 0.0039 "
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 Dunethyl PHOSPHATE Ce,[(CH,),P04]8.H,0.
100 gms. H^ dissolve 79.6 gms. Ces[(CHt)sP04]« at 25® and about 65 gms. at
95^* (Morgan and James, 19x4^
u
u
f<
MS
GBBIUM SlUBNATB
OBUUM 8SUNATI Cei(Se04)a.iiHA
Sqlubiuty in Water. (Gngohni* 1908.)]
Gfltt.
r. a»(Seooa«
zoo Gins. HjO.
Solid Phase. 1*.
Gma.
Cet(SeOi)f
perxooGma.
EW).
0 39SS
Cei(Se04)s.i2HsO 60
13.68
II. 6 37.0
60.8
13.12
12.6 36.9
CdCSeOOs-iiHiO 78.2
5-53
26 33.84
80.S
4.56
28.8 33.22
91
2.02
34.2 331S
Cei(Se04)s.ioHiO 95.4
1.536
45 32.16
98
1.785
45-9 31 89
" 100
2.513
Solid
Cei(Se04)t.8I^
ti
It
Cc^(Se04)8.7HiO
it
Ce^(Se04)t.4H^
tt
tt
CESIUM SULFATE Cei(S04}t.
Solubility of thb Sbvbral Hydrates in Water.
(Koppd, 1904; the preyious detennioatioDS by Muthman and Rolig» zSgS* and by Wyioubofl, 1901,
axe ahown by Koppd to be ioaocuiate.)
Gms.
. Cei(S04)j
t*. per 100
Gms.
Solution.
o 14.20
18.8 14.91
19.2 15.04
Mols.
^^M*Jli!" SoBdPh.se.
HaO.
Gms. Mols
Gms. *
Solution.
HaO.
Solid
O
IS
21
31.6
45-6
50
60
65
o
IS
17 -35
10.61
8.863
6.686
4.910
4.465
3-73
3-47
15-95
9-95
0.525
0.555
0.561
0.665
0.376
0.308
0.227
0.164
0.148
0123
0.114
0.605
0.350
Ces(SOi)s.iaH^
Ces(SO«)i.9HiO
Ce^SQ^JSB^
20.5
40
60
45
60
80
100.5
35
40
50
65
82
100.5
8.69
5-613
3-83
8. 116
3-145
1. 19
0.46
7.8
5-71
3-31
1.85
0.98
0.42
0.302
0.188
0.129
0.280
0.103
0.0382
0.0149
0.27
0.19
o.ii
0.06
0032
0.014
O^SO^SB^
••
Gei(SQJ..5H^
Cei(SQi)t^EbO
In aq. boIs. of
K1SO4 at i6'.
Gms. per 100 Gms. IW).
S5Z
In aq. sols, of
(NHOiSO* at i6*.
Gms. per xoo Gms. HiO.
SOLUBIUTY OF CerIUM SULFATE IN AqUEOUS SOLUTIONS OF AlKALI
Sulfates. (Bane, xgxo.)
In aq. sols, of
NasS04 at 19*.
Gms. per 100 Gms. H»0.
NatSOi. Ce»(SOi)».
o 9.648
0.328 0.637
0.684
1. 091
1.392
1.699
2.640
3.589
5.660
7.710
The following double salts were found.
3K,S04.8H,0. Ce,(S04)..5K,S04, Cei(S04)^NaiS04.2H,6, 'Cei(Sd4)»(NH0iS5i
8HsO and Cei(S04)t.5(NH4)iS04.
o
0.178
0.510
0.726
1.290
o
Cei(S0i)«.
10.747
0.956
0.432
0.250
0.042
6.949 (at 33*)
(NHOsSa.
o
3 464
9 323
19 . 240
29.552
45.616
55 083
63.920
72.838
0.259
0.0937
0.0570
0.0303
0.0120
0.0065
0.0046
0.0037
Cei(S04)i.KiS04.2H,0. 2Cea(S04)i,
Cc^SOOi.
10.747
1.026
0.782
0.748
0.701
0.497
0.194
0.090
0.035
OKBIUM SULFATE
244
Solubility of Cerium Sulfate in Aq. Solutions of Sulfuric Acid at 25*.
(Wirth. Z9xa.)
Normality
of Aq.
HsSOi.
0.0
O.I
I.I
2.16
Gms.
ICO Gms.
t. Sol.
Solid
Phase.
CeOi - Ce»(Sa)».
4 . 604 7 . 60 Cei(S04)|.8HdO
4.615 7.618
3.64 6
3.04 5.018
CERIUM SULFONATES.
Solubility in Water.
II
«
Normali^
of Aq.
HiSOi.
4.32
6.685
9.68
IS IS
Gms. per xoo Gms.
. Der
Sat.
Sol.
Solid
Phase.
CeOi - Ces(S04)s.
2 3-301 Cei(S0J,.8H^
O.9II5 1.505
0.4439 0-733
0.145 0239
II
M
M
(Holmbeig, 1907; Katz and James, 19x3.)
Name.
Cerium m Nitrobenzene Sulfonate
Fonnula.
15
Gms.Anhv-
drouaSalt
per zoo
Gms. HsO.
25. 5
S.89
f.
nyazuus osui
per zoo Gms.
Sat. Sol.
Solid Phase.
2S
0.005
Co,(QHA).4iH^
20
0.7
Cei(C«H«0J|.6Hd0
20
2
II
20
0.4
M
20
0.2
M
CerCJl4(NCWSO»lt.6H,0
Cerium Bromonitrobenzene Sulfonate Ce[C6H|Br(NQi)SC)»i.4.2]t.8HsO 25
CEBIUM TARTRATE Cet(C4H40«)«.4iHsO, also 6H2O.
Solubility in Water (Rimbach and Shubert, 1909, by electrolytic method)
AND in Aq. Solutions. (Hohnbeig, 1907.)
Gms. Ao-
Solvent.
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.
CERIXTM TUNGSTATE Ce2(W0«)«.
Freezing-point lowering data for mixtures of Cei(WOs)s and PbWOi are given
by Zambonmi, 1913.
CETTL ALCOHOL Ci.HnOH.
100 gms. methyl alcohol dissolve 96.9 gms. CuHtOH at 23.9®. CTimofeiew, 1894-)
'^ ethyl " " 102.2 " " " "
I* «« U *t ^jQ ** " ** ^m U
propyl " " 405 " " " 39
CHLORAL H7DRATE CCU.CHO.HsO.
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.
'w. ' S. '
In Chloroform.
'w. S. '
In Tol
Inene.
w . r
W.
s*.
s:
0 ]
1-433
189.7
I. II
"33
I -53°
3-7
0.898
3-2
s ^
[.460
233 0
1. 16
130.0
•515
4.0
0.900
4.0
10 ]
[.435
275.0
I 23
140.0
Sio
S-o
0.910
7.0
IS 3
C.510
330 0
I 30
160.0
•SOS
9.0
0-915
II. 0
30 ]
t-53S
383 0
1.36
185.0
.510
19. 0
0.94
21.0
25 J
fS55
433 0
1.42
215.0
.520
340
0.97
36.0
30 3
[.580
480.0
1-49
245.0
S40
56.0
1.02
56.0
35 3
t-59
516.0
1-55
280.0
570
80.0
I 13
80.0
40 ]
[.60s
• . ■
1.60
320.0
S90
IIO.O
1.40
IIO.O
45 3
[.620
• • •
...
■ • •
1 . a
...
a a •
• . •
W = wt. of I cc. saturated solution, S
grams solvent.
Gms. CaHQ,.HaO per loo
245 CHLORAL HYDRATK
Solubility in Several Solvents.
p I _. *• Gms. CC1»C0H.H*0 c«i^„f ♦• Gms. CCliCOH.IbO
Solvent. r. per loo Gms. Solvent. =>oiveni. «. loo Gms. Solvent.
50% Aq. Pyridine 20-25 374 (Ddm, 1917.) Ether ord. t. 200 (Squires.)
P3rridme 20-25 80.9 " Oil tur- { cold 10 "
Carbon Disulfide ord. t. 1.47 (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 (1Q08) ; 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 Solvent*. t. Dist. (M. Con^''^, golvent. Authority.
Water and Ether 0-30** u
Water and Benzene
Water and Olive Oil ord. 4
" " " 30* 4
" " " 3 16
" " Toliiene 0-20** 58-74
235 (Hantzach and Vagt, xgox.)
(Bubanovic, 19x3.)
9 (Baum, X899.)
3 (Mqrer, xgox; X909.)
7 (Meyer, X90X.)
5 (HantzBch and Vagt, xgox.)
CHLORAL FOBMAMIDE CCU.CH(OH).NH.CHO.
100 gms. H,0 dissolve 5.3 gms. CCUCH(OH).NHCHO at 25*. (U. S. P.)
100 gms. 95% alcohol dissolve 77 gmsJCCl,CH(OH).NHCHO at 25*.
CHLORINE Cli. Solubility in Water.
(Winkler, 19x2; Roozeboom, 1884, 1885. x888.)
Solid Phase.
Ice + C1.8 aq.
C1.8 aq.
ti
u
((
u
ct
it
" + 2 layers
r.
^'.
«•
r.
Gms. U per
xoo Gms. ftO.
0
4.610
1.46
—0.24
0.492
3
3-947
I -25
0
0.507-0.560
6
3-4II
1.08
2
D.644
9
3 031
0.96
4
0.732
9.6
2.980
0.94
6
0.823
12
2.778
0.88
8
0.917
10
3 095
0.980
9
0.965-0.908
IS
2.63s
0.83s
20
1.85
20
2.260
0.716
28.7
369
25
I -985
0.630
30
1.769
0.562
40
1. 414
0.451
SO
1.204
0.386
60
1.006
0.324
70
0.848
0.274
80
0.672
0.219
90
0.380
0.125
100
c
0
ff « vol. of CI .(reduced to o® and 760 mm.) absorbed by i vol. HjO at total pres-
Bure of 760 mm.
a » Gms. CI per 100 gms. HsO at a total pressure of 760 mm.
The coefficient of solubility of chlorine at 15®, determined by an aspiration
method, is given as ^1.7 for carbon tetrachloride, 39.6 for acetic anhydride, 36.7
for 09.84.% acetic acid, 25.3 for 90 vol. % acetic acid, 16.43 for 75 vol. % acetic
acta ana 13.45 for 65 vol. % acetic acid. (Jones, x9xx.)
OHLOBINI 246
Solubility in Water.-
(Goodwin, 1883.)
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
obtain^ for solutions in contact with much, little, or no chlorine hydrate. The'
following results are taken from an average curve:
r.
SolubiUty
Coeflkient.
2-5
1.76
5
2
75
2.25
10 .
2.7
r.
Solubility
Coefficient.
f.
stability
Coefficient
II
3
25
2.06
12. s
2.7s
30
1.8
IS
3.6
40
1-35
20
2-3
so
I
solubilitt of chlorine in aqueous solutions op hydrochloric
Acid and op Potassium Chloride.
(Goodwin.)
Coefficient of Solubility in:
_^ Results at 2]
Gms. Helper
[^ (MeIlor,z9oz.)
**• ' HQ. HCl
na
KQ
Solubility of O.
(x.046 Sp. Gr.). (z.08 Sp. Gr.). (x.
i25Sp.Gr.).(3G
g.perzoocc.) xooocc' (Ostwald/,seep.as7.)
0 4.1 6.4
7-3
IS
0.
2.2799
S S-I S.2
6.7
2
3 134
1.6698
10 4.1 45
6.1
2.2
9.402
1-5013
IS 3-5 3-9
S-5
1.6
12.540
1.5292
20 3 3.4
4-7
1.2
31 340
1-8033
25 2.S 3
4
I
125.360
2.4473
30 2 2.4
• • •
0.9
219.380
3-I312
40 1.25 1.6
• • •
• . •
313-401
3.8224
' Goodwin also gives results for solutions of NaCl, CaCls, MgCls, SrCli, FetCls,
C0CI2, NiCli, MnCls, CdCls, LiCl, and in mixtures of some of these, but the con-
centrations of the salt solutions are not stated.
Solubility op Chlorine in Aqueous Solutions op Sodium Chloride.
(Kumpf, x88s; Kohn and O'Brien. X898.)
r.
Coefficient of Solubility in:
9.97% NaCL
x6.ox% NaCl.
19.66% NaG.
36.39% NaG.
0
2.3
1-9
1.7
o.S
S
2
1.6
1.4
0.44
10
1.7
1-3
1. 15
0.4
IS
1.4
1.06
0.95
0.36
20
1.2
0.9
0.8
0.34
25
0.94
0.7s
0.6s
0.3
50
...
...
• . •
0.2
80
* * * .
...
• • •
0.05
100 cc. of 6.2 per cent CaCls solution dissolve 0.245 gm. Cl at 12^.
100 cc. of 6.2 per cent MgCls solution dissolve 0.233 8^^*- Cl at 12®.
100 cc. of 6.2 per cent MnCU 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 Mdntoth. 1916.)
+ Ethyl Alcohol " «
4- Methyl Alcohol *•
4- Ethyl Acetate (Waeatag and Mdntoah, 1916; Maass and Mcintosh, 191a.)
" 4- Methyl Acetate (Waentig and Mclntodi, 19x6.)
4- Ether
+ Hydrochloric Add (ICaaas and Mcintosh, 1919.)
" + Iodine (Stortenbecker. 1888, 1889.)
" 4* Sulfur (Ru£F and Racher, 1903.)
" 4- Sulfur Dioxide (Smits and Hoay, 19x0; Van der Goot, 19x3*)
4- Sulfuryl Chloride (SOiCls) (Van der Goot, 19x3.)
4- " " -f Sulfur Dioxide
4* Stannic Chloride (Waentig and Mcintosh, 1916.)
4* Toluene (Waentig and Mcintosh, 19x6; Maass and Mcintosh, X9X3.)
4- Nitrosyl Chloride (NOCl) (Boubnoff and (kiye, X9XX.)
Distribution of Chlorine Between CCU and Gaseous Phase and
Between CCU and Water.
(Jakowbin, X899.)
Results for CCU + Results for dist. between CCI4 and HiO.
Gaseous Phase. ist Series. 2nd Series.
Millixnols per Liter. Millimob per Liter.
MiDunolsQ per Liter. / *^
^^^y^^- CCI4. IfaOIayer. ^ ^^
Gaseous CCI4 Total • Unhydro- T-yer Total Unhy- Laver
Phase. Phase. Q. lixed Q. ' Q. diolized a '
O.IIO9 8.908 58.21 39.67 803.3 61.73 42.5s 864.2
0.2666 22.46 38.36 22.97 464.6 42.62 26.36 335.1
0.5365 44.14 23.08 II. 12 222.5 28.98 15.24 311. 3
0.8800 75.09 10.10 2.707 52.93 21.70 9.94 202.7
Data for the effect of HCl upon the distribution between HiO and CCI4 are
also given.
CHLORINE DIOXIDE C10i.8H^ =b iHsO.
Solubility in Water.
(Bray, 1905-06.)
*•• ^i^ SolidPhase. f. Gms^C^ SolidPhase.
— 0.79 Eutec. 26.98 QOtJSBfi-\-lcc 15. 3 87. 04 OOt^njO±xBfi
0 27 . 59 CiOtJSHfi±iBfi 10 . 7 tz. pt. 107 .9 " + liquid 00^
1 29.48 '* 14 mofe than > 107.9 liquid QOh
5.7 42.10 " 10.7 116. 7 "
10 60.05 " X inorethaii> 108.6 **
The exact composition of the hydrate could not be determined on account of
manipulative difficulties.
Data for the distribution of ClOs between HsO and CCI4 at o^ and 2^** are given,
also some results showing the effect of HsS04, KClOt and of KCl on this distribu-
tion.
CHLORINE MONOXIDE ClsO.
100 volumes of water at 0° absorb 200 volumes of CliO gas.
CHLORINE TRIOXIDE CIA.
Solubility in Water at Approx. 760 mm. Pressure.
(Brandan, 1869.)
r. 8.5*. 14*. ai*. 93*.
Gms. CIA per 100 gms. HsO 4.765 5.012 5-445 5-651
Garzarolli and Thumbalk, 1881. say that CIA does not exist, and above
figures are for mixtiues of ClsO and CI.
CHLOROFORM 248
CHLOROFORM CHCU.
Solubility in Water.
(CfaAocd and Parmentier, 2885; Rex, 1906.)
^ Gms. CHCIa per Density of ^ Gnu. CHCb jE«r
* * Liter of SolutMn. SolutaoBS. ' xoo Gms. H1O (Rei).
o 9.87 X. 00378
3.3 8.90
17.4 7.12 X. 00284
29.4 7.05 X. 00280
41.6 7.12 1.00284
54-9 7.75 1.00309
,^'100 cc. HiO dissolve 0.42 cc. CHCU at 22®; Vol. of sol. == 100.39 cc-» Sp. Gr. =
1.0002.
100 cc. CHCU dissolve 0.152 cc. HiO at 22®; Vol. of sol. = 99.62 cc., Sp. Gr. =»
1. 483 1. (Hers, X898.)
Solubility op Chloroform in Aqueous Ethyl Alcohol, Methyl
Alcohol, and Acetone Mixtures at 20°..
(Bancroft, 1895.)
0
1.062
xo
0.895
20
0.822
30
0.776
In Ethyl Alcohol.
In Methyl Alcohol.
In Acetone.
PersccCflHiOH.
Per 5CC.
CHiOH.
Pers cc
ccHiO.
. (CHi>tC0
cc. IU>. cc. CHCIs:
cc. HsO.
cc CHCU:
. cc. CHOi:
XO 0.20
10
O.IO
5
0.16
8 0.3
S
0.48
4
0.22
6 0.515
4
0.8
3
0.33
4 X.X3
3
4
2
0.58
2 2.51
X.49
7
I
0.955
X ' 4.60
1.35
8
0.79
1. 12
0.91 5
X.I2
xo
0.505
1.60
0.76 6
0.30
250
0.55 8
0.21
3.50
0.425 10
0.19
4
0.20 20
0.16
5
0.125 30.24
0.12
10
Data for the system chloroform, ethyl ether and water are given by Jfittner,
1901.
Experiments by Schachner (1910) show that various fats (olive oil, sheep suet,
goose fat) in an atmosphere containing 0.55% CHCU vapor, dissolve o.9^h>.98
per cent CHCU at 38.5 .
Data for the properties of solutions of CHCU in water, saline solution, serum,
hemoelobin, etc.,4n 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 (Mmss and Mcintosh, 1912.)
" + Hydrochloric Acid (Baume and Borowaki, 19x4.)
+ Methyl Alcohol
" -j- Methyl Ether (Baume, 1914, 1909.)
' p nitrophenyl chloroform + m nitrophenyl chloroform (Holleman, 19x4.)
CHOLESTKROL C»H«OH.H,0.
100 gms. H2O dissolve 0.26 gm. cholesterol at 20-25^ (Dehn,x9x7.)
pyridine " 68.10 gms.
50% aq. pyridine " i . 10 " " " " ' "
100 cc. HsO dissolve 0.0006 gm. cholesterol-di^tonide at b. pt. (Mueller, 19x7.)
100 cc. ether dissolve 0.0007 g^- 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, 191 1.
249 CHOLESTEROL
Solubility of Stearic Acid Ester of Cholesterol in Oils at 37® and
Vice Versa. (Paehne, 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 tne melting point.
^ „ . Gin9.0florAddperioo
Sdveot. fof ^^r^ c^, ^ Gma. Sat. Solution in
Sp. Gr. M. pt.
Olive Oil 37.6 3.3s Olive Oil 25.5 33.8
Castor Oil 37.6 0.26 Oleic Add 37 40
Oleic Add 37.5 4. 11 Castor Oil 5 1.85
Ricinic (Oil) Add 37 0.33 RidnicAdd 20 16
Pseudo Ricinic Add 36 . 2 0.85 Pseudo Ricinic Add 10 12
Crotonic (Oil) Acid 36.5 0.87 CrotonicAdd (5) $
CHOLnnS PEBCHLORATE and its Nitric Ether.
100 gms. H,0 dissolve about 290gms. (CH,),N(Cl04)CHjCHj.0Hat i5°.l(Ho£mann
100 gms. H2O dissolve 0.62'gm. (CH,),N(C104)CH,.CH,.0N0« at 15*. [ hJ£^m
100 gms. HjO dissolve 0.82 gm. " at 20**. J ign.)*
CHROMIUM ALUMS.
Solubility of Chromium Alums in Water at 25**. (Locke. 1901.)
Per ICO cc. Water.
Alum. Fonnula. Grams Grams Gram'
Anhydrous. Hydxated. Mols.
Potassium Chromium Alum K2Cr2(S04)4.24H20 12.51 24.39 0.0441
Tellurium Chromium Alum TeaCr2(S04)4.24HiO 10.41 16.38 0.0212
CHROMIUM CHLORIDES CrCl«.6H20.
Solubility of the Green and the Vicm^et Modifications in Water at 25*.
(Olic 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
bv precipitating with silver nitrate. A freshly prepared solution of the green
chloride fields only one-third of its chlorine in the cold, hence the composition of
this modification, according to Werner, is represented by the formula' [Cr(HsO)4Clt]
C1.2HtO. The violet chloride is considered to have the composition, [Cr(HsO)«]Cl|.
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 CT) 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 oT HCl 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 0° to a thin
mush. This was then agitated at 25° and portions removed at successive inter-
vals of time and analyzed. The results snow the total chloride and per cent
present as the green modification.
25 Gms. Green Salt 25 Gms. Violet Salt 25 Gms. Violet Salt + locc.
+ 10 Gms. HjO. + 10 Gms. HjO. of 35% Sol. of the Green Salt.
Tfaneof
Gins.Crai
Percent
Time of Gms. CrCh Per cent
Time of
Gms.CrCU Pei**cent
\git»-
per xoo Gins.
of Green
AffiUH per loo Gms. of Green
Agita-
per xoo Gms. of Green
tion.
Sat Sol.
Salt.
tion. Sat. Sol. Salt.
tion.
Sat. Sol. Salt.
ihr.
58.36
91-7
Jhr. 61.99 1.53
i}hr.
65.49 15-95
4hrs.
63.27
75-2
I day 63.88 8.46
2 days
70.47 26.81
I day
68.50
62 ..36
4 days 70.68 30.89
s ::
76.38 39-34
3 da3rs
68.9s
57.22
7 " 72.11 37.28
8 "
73.26 34-20
19 days
68.58
57.38
26 " 70.62 51.54
12 "
71.14 58.60
In a later paper Olie Jr. (1907) gives additional results at 29**, 32** and 35*.
100 cc. anhydr . hydrazme dissolve 1 3 gms. CrCU at room temp. (Welsh & Broderson/zs.)
CHROMIUM TRIOXIDE 250
CHROMIUM TRIOXIDE CrO|.
Solubility in Water.
(Btkhner, and Pxini, X9i»-X3; Kzemaiin, Dftimer and Bfrninrh, 19x1; Koppd and Blmncnthal,' X907;
and Myliua and Funk, 1900.)
f nS^^ Solid 4. ^^^ Solid f }^'^ Solid
— 0.9 3.6 loe — 435 491 Ice 50 64.55 CiOb
— 1.9 7.8 " - 60 53.3 " 65 64.83
— 3.7 II. 5 « —155 60.5 "+CiOb 82 66
— 4.8 14. 1 .« — 20 61.7 QOb 90 68.5 «
— 10.95 24.9 " O 62.24 " 100 67.4 «
— II. 7 25.2 " + 18 62.45 " 115 68.4 "
— i8'7S 33-5 " 24.8 62.88 « 122 70.7 -
— 25.25 39.2 " 40 63.50 I93'I96 100 [dccompodtkm
Density of solution sat. at 18* « 1*705.
100 cc. anhydrous hydrazine dissolve i gm. Crd with evolution of gas and
production of a black precipitate at room temp. (Wdah and Bxodefion, X9X5.)
CHROMIUM DOUBLE SALTS.
Solubility in Water.
(J<k|enaen, 1879, 1884, 1890; Stnive, 1899.)
Onti. per
Name of Salt. Fonuila. t*. xooGms.
H«0.
Chloiotetraamine Chromium Chlo-
ride CrCl(NH,)4(0H,)Cli 15 6.3
Chloiopurpureo Chromium Chloride CrCl(NHt)6Cls 16 0.65
Luteo Chromium Nitrate Cr(NHs)6(N0i)i ? 2.6
Chioropurpureo Chromium Nitrate CrCl(NHs)i(NOi)i 17.5 1.4
Chromic Potassiiun Molybdate 3KsO.CriOk.i2MoQi.2oH^ 17 2.5
CHROMIUM SULFATES (ousandic).
SOLUBILITT IN WaTBR.
S^ Gmi. i^^oo Gms. Solid Phase. Authority.
Chromous 1 2 . 35 (at o^) CrS04.7H^ (Moiisan. x883.)
Chromic 120 (at ?^) Cri(S04)i.i8H^ (Etaxd, X877.)
CHROMIUM THIOCYANATI Cr(CNS),.
Data for the distribution of Cr(CNS)i between water and ether at 0^-30^ are
given by Hantzsch and Vagt, 1901.
CHRTSAROBIN CmHuGt.
Solubility in Several S(x.vbnts.
(u. s. p.)
-, Gms. per 100 Gnu. Solvent at; Gnu. per 100 Gmfc
Water 0.021 0.046 Chloroform 5.55
Alcohol 0.324 0.363 (60**) Ether 0.873
Benzene 4 ... Amyl Alcohol 3.33
Carbon Disulfide o . 43
CHRTSINE CuHu.
Solubility in Tolubnb and in Abs. Alcohol.
(v. Becchi.)
100 gms. toluene dissolve 0.24 gm. CisHit at I8^ and 5.39 gms. at 100®.
100 gms. abs. alcohol dissolve 0.097 S^* CuHu at i6^ and 0.170 gm. at boiling
point.
251
CXNEOLK
CXNEOLK (Eucalyptole) CioHuO.
Freezing-point lowering data (solubility, see footnote, p. i) for mixtures of
cineole and each of the K>llowing compounds are given by Bellucci and Grassi,
(19 13); phenol, a and /? naphthol, 0, m and p cresol, o, m and p nitrophenol,
0, m amidophenol, pyrocatechol, resorcinol, hydroquinone, guaiacoi, o, m and p
oxybenzoic acid, methyl salicylate, phenyl salicylate, naphthalene and thymol.
CINCHONA ALKALOIDS.
S(H.UBILITY OP ClKCHONINB, QnCHONIDINB, QuININB, AND QuiNIDINE IN
Several Solvents. (Moiier, 1903; see also Pmnier, 1879.)
Grams of the Alkaloid per 100 Grams Solution.
Solvent.
Cinchonine Cinchonidine
CisHnNiO. CmHssNbO.
Ether
Ether sat with H,0
HjO sat. with Ether
Benzene
Chloroform
Acetic Ether
Petroleum Ether
Carbon Tetra Chloride o .0361
Water 0.0239
Glycerine £i5_j®) o . 50
Quinine
/ * *
Hydrate. Anhydride.
O.IO
0.123
0.025
0.0545
0.6979
0.0719
00335
0.2II
0523
0.0306
0.099
9.301
0.3003
0.0475
0.0508
0.0255
1. 619
5 618
0.0667
o . 2054
100 4-
465
0.0103
0.203
0.574
0.50
0.876
2.794
0.0847
1. 700
100 -f
2.469
0.0211
0.529
0.0506
Quinidine
C»HmN,0,.
0.776
1.629
0.031
2 -451
100 -f
I.761
0.0241
0.565
0.020a
Solubility of Cinchonine and CiNCHONmiNtf in Several Solvents.
Solvent.
Water
Gms. Alkaloid per xoo
fo Gms. Solvent.
Cinchonine. Cinchonidine,
Old. temp. 0.0043
«
Aq. zo% Ammonia
Aq. 85% CiH»OH+io% Am.
Aniline
Pyridine
50% Aq. Pyridine
Aq. 8s% CiEUOH (Ao-0.832)
CaOH ^95%)
CiHiOH (prob. 92.3 wt. %)
Abs. CtHsOH
Abs. CtH^OH
Benzene
Acetone
Chloiofoim
it
a
Ether
20
20
20
20
20
20-25
20
20
25
19
25
25
25
17
25
50
25
32
25
19
25
20
20
0.0I3I
O.OII3
0.025
0.41
1.6
1.4
« • •
0.86
0.80
0.62
0.874
0.89
0.057
0.091
0.014
0.606
0.565
0.055
0.264
1. 10
Z.09
0.785-1. 17
3.5
0.021
Authority.
(Hatcher, 1903.)
(Scholtx, 19x3.)
(Schaefer, 19x0.)
(Scholts, Z9X3.)
M
7 . 78 (Scholta, 19x3; Dehn, 19x7^
10 (Dehn, X9X7.)
(Scholts, 19x3.)
5 (WhenyandYaiiovaky,x9z8.)
5 . z (Schaefer, 1913-)
(Timofeiew, 1894.)
(Sill, X905.)
O . Z 27 (Schaefer, X9X3.)
(Sill, X905.)
(Oudemans, 1873.)
Z9 (Schaefer, 19x3.)
(KOhler, X879.)
(Sill, 1905.)
(KOhler, x879.)^
(Sill, 1905.)
(Timofeiew, X894.)
(Schaefer, X9X3; Sill, 1905.)
(Scholtz, X9X3.)
7.39
Isoamyl Alcohol '
Isobutyl Alcohol
Meth^rl Alcohol
Pipendine
Diethyl Amine 20 z.3
Results for the solubility of cinchonine and cinchonidine in mixtures of ethyl and
methyl alcohols with benzene and with chloroform are given by Schaefer (191 3).
It 18 pointed out by Schaefer (191 o), that if the saturated solution is analyzed
by shalang out with chloroform or ether, variable results, depending on the age
and methoid 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 obtain^l by agitating at mtervals, instead of constantly at the given
temperature.
dNCHOHA ALKALOIDS 253
Solubility op Cinchoninb, Cinchonidinb and Cinchotinb Salts in Watbs.
Gms. per lop Gma. HgO.
Sah. f. Cincbonine Oncbom- Ciocbodne Authority.
Sfth. dine Salt. Salt.
Hydiobromide 2$ 1.7 i-66 ... (Sdnefer. tgio.)
Bmydiobromide 35 55.5 14 -3 ••• "
Hydrochloride 25 4.5^ 4.8* s.za* (Scfaaefer. xgio: FontandBflhrinfler. 1881.)
Bihydrochloride 25 ... 62.5 ... (Schaefer. 1910.)
Sulfate 25 z . 17^ 1 . 08^ 3 . 28* (Schaefer, 19x0: Font and Bfihrioger. 1881.)
Sulfate 80 3.1 4.8 ... (U.S. P.)
Bisulfate 25 66.6 100 ... (Schaefer. 19x0.)
Perchlorate Z 2 0 . 3(sohrent -aq. 6% HCIO^ (Hofmann. Roth. Hflbold and MeUler, 1910.)
Salicylate 25 0.17 0.075 ... (Schaefer, 19x0.)
Tannate 25 0.091 0.055 ••• "
Tartrate 25 3 . Z2' ... z . 76* (Schaefer. 1910: Forst and Bdhiinger, 1881.)
Bitartrate z6 0.99 Z.28 (Forst and Bdhiinger. z88x.)
Oxalate 20 0.96 ... z.i6 " "
* 4.16 at lo*. « 4 at IS*. • at lo*. * i.sa at 13*. » i at 15*. • at ij*. » 3 at x6*. • at i6*.
Solubility op Cinchoninb Sulfate and of Cinchonidinb Sulfate in
Alcohol and Other Solvents.
Gma. per xoo Gms. Solvent.
Solvent f. rc^H-N^V (C»H«N.0V Authority.
».^^. '^^.^.
Ethyl Alcohol (92.3 wt. %) 25 9.8 (10) 0.85 (1.4) (Schaefer, 19x3; U. S. P.)
" " ** 60 ...(19.2) ... (3.1) (U.S. P.)
Methyl Alcohol 25 83.9 35.9 (Schaefer, 1913; U. S. P.)
Chloroform 25 0.66 (z. 45) o.z (o.zz) (Schaefer. 19x3; U. S. P.)
Ether 25 Q.04 0.02 (U.S. P.)
Glycerol Z5 6.7
Results for mixtures of alcohol, chloroform and benzene are given by Schaefer, 'l 3.
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 ACm C«H|CH:CH.C(X)H.
100 gms. H2O dissolve 0.0495 gm. C«H»CH iCHCOOH at 25*. (De Jong, 1909.)
100 gms. HiO dissolve 0.0607 gm. CeH»CH :CHCCX)H at 25*. (Sidgwick. X910.)
100 cc. 0.5 n sodium cinnamate solution dissolve 0.155 gm. QHiCH :CHCOOH
at 25^ (Sidgwick. 19x0.)
100 CC. sat. sol. in petroleum ether (b. pt. 30^-70®) contain 0.095 gm. CeHiCH :
CH.C(X)H at 26^
100 cc. sat. sol. in carbon tetrachloride contain 2.172 gms. CtHiCHiCH.COOH
at 26^. (De Jong. 1909.)
100 cc. sat. sol. in 95% formic acid contain 3.76 gms. C«HiCH:CH.COOH at 20^.
(Aschan. 19x3.)
Solubility of Cinnamic Acid (Melting point, 133®) in Alcohols. (T!niofeiew.x894)
Gma. Cinnamic Acid per xoo Gms. Sat. Solution in:
r.. , • .
CH/)H. CiHiOH. CHtOH. (CH^,CH.CH|0H.
— 18 8.1 6.74 4.3
-12.5 9.3 8 5.5
o 13 II. 3 8.2
+ 19.5 22.5 18. 1 13.4 8.6
Solubility of Cinnamic Acid in Organic Solvents at 25^. CHeizand Rathmann. 19x3.)
Gms.C|jig
Gms. C^CH: Solvent. Gms. C»H«CH: Solvent CH:CH-
Solvent. CHC(^««; u^p. ' rn' CHC&l ger . ^^^ " ' „^^ COOH
xoo cc. Sat. Sol. ^**t.J| v^CU xooccSat.Sol.(>iH<-^ C|HCU per xoo cc
Sat. SoL
Chloroform 12.09 ^oo cc.+ o cc. Z2.09 zoo cc.+ o cc. 6.04
Carbontetrachloride z.75 80 "+20 " 9.86 80 "+20 " 5.9Z
Trichlorethylene 6.04 50 "+50 " 6.6z 50 "+50 ** 5.85
Tetrachlorethylene 2.55 333 "+66.6" 4.50 33.3 "+66.6" 5.8a
Tetrachlorethane zi.05 20 " -j- 80 " 3.32 20 "+80 " 5.70
Pentachlorethane 5.54 o " +100 " 1.75 o " -j-zoo " 5.54
353 CniNAMIC ACID
OIHHAMIO AOID C«H5CH:CH.C00H.
Solubility op Cinnamic Acid in Aqueous Solutions op Sodium
acbtatb, butyrate, formate, and salicylate at 26.4**.
(Philip — J Chem. Soc.87f o^a, '05.)
Calculated from the original results, which are given in terms of
molecular quantities per liter.
Gms NaSalt Gms. C«HgCH:CH.COOH per liter in Solutiona of;
per Liter.
CHaCOONa.
CiHrCOONa.
HCOONa. C«H«.OH.COONa.
0
0.56
0.56
0.56 0.56
I
I SO
1.30
092 0.62
2
2.12
1.85
1. 12 0.70
3
2.52
2.25
1.27 0.73
4
2.85
2.60
1.40 0.77
5
3 OS
2.90
1.47 0.80
8
• • •
• • •
... O-QO
z liter of aqueous solution contains
0.491 gm. C<^,CH:CH.COOH
at 25^ (Paxil).
,
Grams per
Liter.
'CaH«CHsNIis.
C6UfiCH:CHCOOH.'
0
0.49
I
I 52
2
2.20
3
2.83
4
3-35
3.80
Solubility op Cinnamic Acid in Aqueous Solutions op Anilin
AND OP Para Toluidin at 25®.
(Loiwenherz — Z. physik. Chem. as* 304, '98.)
Original results in terms of molecular quantities per liter.
In Aqueous Anilin. In Aqueous p Toluidin.
Grams per liter.
£ANH» QgOsCHzCHCOOHl
o 0.49
Z Z.20
2 Z.65
3 2.02
4 2-35
6 2.92
Treezin^-pc^t data for mtxtures of cinnamic acid and dimethylpyrone and
for hydrocinnamic acid and dimethylpyrone are given by Kendall, 1914.
BromoCINNAMIC ACIDS.
Solubility op a and op fi Bromocinnamic Acids in Water at 25^
(Paul, X894.)
. . . For xooo cc. Sat. SolutioiL
Add.
aCaftCHiCBrCOOH
/SCeUCBnCHCOOH
Solubility op a Iso Bromocinnamic Aero in Aqueous Solutions op
OxANiLic Aero (Melting point =- 120*) at 25^
(Noyes, 1890.)
Normality oi Solutions. Grams pjcr Liter.
C|H«NHCO- C,H»CH-,
COOH. CBrCOOH.
o 3.99s
4. 54 3178
8.65 2.928
' Cms.
3 9325
0.5255
MilKmnb.
17.32
2-315
CH.NHCO.
COOH.
CH,CH-
CBtOOOH.
0
0.0176
0.027s
0.0140
0.0524
0.0129
CINNAMIC ACIDS
254
Alio 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:
Allocinnamic Acid
of M. pt. 68^
(Meyer, 191 1.)
Allocinnamic Acid Allocinnamic Acid
of M. pt. 58**. of M. pt. 42^
(Natund iffft^nnamii' Add.) (Artifidal laocumaxnic Add.)
Melted Allocin-
namic Acid.
18
35
45
55
Gms. Add
per Liter.
6.88
8.4s
II. 14
14.46
18.4s
18
25
35
45
Gms. Add
per Liter.
7.62
9-37
12.39
16.09
f.
18
25
35
Gms. Add
per Liter.
8-95
11.03
14.61
f.
18
25
35
45
55
65
75
Gms. Add
per Liter
13 63
14.44
16.05
18. II
20.55
23-43
27.69
These curves intersect that for the melted acid at the
melting points of the solid isomers.
The results show that the three isomers are polymorphic modifications of the
CIS acid.
100 gms. ligroln (b. pt. 60-70^) dissolve more than 16 gms. isocinnamic acid.
(Liebemuum, 1903.)
100 gms. ligroln (b. pt. 60-70^) dissolve approx. 2 gms. allocinnamic acid. "
Solubility of a Chlorocinnamic Acid, Etc., in Benzene.
(Stoermer and Heymann, 19x3.)
Gms.
Gms.
Name of Compound.
M.pt.
f.
Cmpd. per
100 Gms.
Name of Compound.
M.pt.
AM Cmpd. per
• • 100 Gms.
a Chlor- 1
137
20
2.6
fi Brom-
13s
13 1.58
AUoa "
III
21
II
AUo /? "
•
159. 5
14 0.86
a Biom-
AUoa "
fi Chlor-
cin-
namic
Add
131
120
142
20
18.
17
S.17
S 6.9
1.94
cis Dichlor-
trans "
cis Dibiom-
on-
namic
Acid
121
lOI
100
13 6.1
14 21.2
14 26.9
AUo/3 "
132
16
3.17
trans "
136
14 10.6
Freezing-point Data (Solubility, see footnote, p. i) for Mixtures of Cin-
namic Acid and Other Compounds, and op Cinnamic Acid Derivatives
AND Other Compounds.
Cinnamic Acid -f- Phenylpropionic Acid (Bnmi and Gomi, 1899.)
p Methoxycinnamic Acid -|- Hydroquinone (de Kodc, 1904.)
a Monochlorcinnamic Aldehyde + a Monobromdnnamic Aldehyde (KOster, 1891.)
Cinnamylidine -h Diphenylbutadiene (Pascal, 1914.)
4- Diphenyldiacetylene "
II
CITBIC ACm (CH,)aCOH(COOH)..H,0.
Solubility of Hydrated and of Anhydrous Citric Acid, Determined
Separately, in Aqueous Solutions 'of Ethyl Alcohol at 25**.
(Sddell, 1910.)
Results for Hydrated Citric Acid. Results for Anhydrous Citric Acid.
0
1. 311
67.5
20
1.297
62.3
20
1.286
66
40
1.246
59
40
I 257
64.3
60
1. 190
54.8
50
1.237
63 -3
70
1. 160
52.2
60
1. 216
62
80
1. 120
48.5
70
1. 192
60. 8*
90
1.065
43-7
80
1. 163
58.1*
100
1. 010
38.3
90
1. 125
54-7*
100
1.068
49.8*
* Solid phase dehydrated moce oc
leas completdy.
Amjd Acetate of *,-o.87so
0,8917
,,
Amy! Alcohol of .(,-0.8170
0.8774
Ethyl Acetate of dn— 0.8915
0.9175
Ether (abs.) of dB-0.7110
o.7"8
Chlorof<mDof da"!. 476
I -4850
355 CITBIG ACm
Scx.UBU.mr of Hvdratbd and of Anbvdsous Citbic Acid, Deterioned
Separately, in Sbvebal Organic Acids at 35°. (Sddeii. 1910.)
Results for Hydrated Citric Acid. Results for Anhydrous Citric Add.
9S0 AmylAcetate 0.S861 4.33
430 Ether (aba.) 0.7160 1.05
176 Chloroform 1.48S0 o
174 Crfl,, CS,
007 CO, or CiHtCH, ... o
100 gms. 95% formic add dissolve 12.35 S'""' citric acid at 30°. (Aochu, 1913.)
lOOgms. (^chiorethylene dissolve o.OosgjD. citricaddatis". CWeiicr&Btiiiiu,'i4J
'^ trichlorethylene " 0.012 " " " " '' . "
" methyl alcohol " 197 gtaa. " " " 10°. Crbno^cinr, 1914.)
" propyl alcohol " 62.8 " " " " . "
DiSTKiBunON OF Citbic Acid between Water and Ether. (Knunr, 191s.)
Results at 15°. , Results at 25.5*.
Hob. Citric Acid per Liter. ^. Mob. Otric Acid pa liut. ^
laSfiLtya. InSttKrUyct. ""■ ""' InH,OUyer. In Ether Larct. """*'■
0.903 0.0077 ^^7 ^'9^75 0.0063 tI4
0.460 0.0036 138 0.481 0,0031 155
0.130 0.0017 1^9 0.341 0.00155 15s
0 . 297 0 . 0033 1 39 0.315 0 . 0080 158
COBALT AHIN18.
Solubility in Water at Ordinary Temperatttre. (Ui De, 1917)
Cnw. Ikmb-
Nvne ol iHineride. Fonnuk. eiide per
HUrSkt-SoL
Triamine Cobalt Nitrate [(NH,),CoCNOi).] a. 883
i.a Dinhrotetraamine oobaltitaranitrodi- f- CN0.)i1'_r„ (NOO,"]' ^
amine cobaltiate L (NH,)J L (N^jJ ^
1.6 Dinitrotetraamine cobaltitetrajijtrodi-
amine cobaltiate " " 0.39S
Hcia-Bimne cobaltihexaiutrooob<iate [Co(NHi)«]>ii— [Co[NOi)i]ni o.oais
COBALT DOUBLI 8ALT8.
Solubility in Water.
sn — J.pr.Chmn.W iS,»],'78i i!»,4^'7o; Knmnkoa— J. nui. phji. cheia. Gca. 14, A*g,
Chloro purpureo cobaltic bromide
Bromo purpureo cobaltic bromide
Chloro tetra amine cobaltic chloride
Chloro purpureo cobaltic chloride
Chloro purpureo cobaltic chloride
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
143
0-467
16
0.19
"■SO
0
0.33"
IS5
0.41
466
1.03
0
4.J6
46.6
"74
0
16. la
16. a
a4.87
19.1
a.o
■S
las
173
0.75
16
0-36
COBALT AGITATI 256
COBALT ACETATI Co(CH,C(X))s.
100 cc. anhydrous hydrazine dissolve i gm. cobalt acetate with evolution of
gas at room temp. (Wdsh and Biodenon, 1915.)
COBALT BROBODE CoBri.
Solubility in Water.
(Etaid, X894.)
t*. 59*. 7S*. 97*.
Gms. CoBfs per 100 gms. solution 66 7 66.8 68.1 (blue)
100 gms. methyl acetate (du *- 0.935) dissolve 10.3 gms. CoBri at i8^
duoi sat. solution >■ I.013. (Naunuum, z9o9-)
COBALT CHLORATE Co(C10i)t.
Solubility in Water.
(Meuaaeii 1902.)
Gms. Mob. Gms. Mols.
(^m, SoKdPhMe. f. Co(a(W, C«(m Solid Phue.
per zoo per zoo u-ms. per zoo
M<^. H|0. Solution. Mdls. H|0.
3.41 loe 18 64.19 14.28 CoCaO^t^H^
9.08 Co(CKW«.6H^ 21 64.39 1451 "
9.20 " 35 67.09 16.10 "
10.7s " 47 69.66 18.29 "
12.90 •• 61 76.12 25.39 •
Density of solution saturated at 18^ » 1.861.
COBALT PerCHLORATE Co(C104)s.9H,0.
Solubility in Water.
(Goldblum and Terlikowaki, z9Z3.)
Gms. Gms.
f.
Co<aa)i
per zoo Gms.
Solution.
— 12
29.97
— 21
53.30
-19
S3 61
0
57.45
10. s
61.83
r.
Co(C10^,
per 100
Gms.H^.
Solid Phase.
f.
gSl3.^^S^' SolidlW
Gms. H|0.
—10.9
32.67
loe
0
1.564 100 OKPO^rSBfi
-30.7
58.16
«
7-5
1.566 101.9 "
~62.3£utec
• • •
Ioe+Co<a04)..9H^
18
1.567 103 -8 ••
-30.7
83.2
Co(a04),.9HdO
36
1. 581 113. 4 *
— ai.3
90.6
M
45
1.588 115 S
COBALT CHLORIDE Cu^u.
Solubility in Water.
(Etaxd — Compt. rend. 1x3, 699, 'pz; Ann. chim. phys. [7] a» 537, '94.)
Gms.
Solid ^o CoOjiper SoUd
Phase. * * 100 Gms. Phase.
Solution.
Coa,.6H,0 (red) 35 38.0 CoCl,.BLO (violet)
" 40 41.0 "
SO 470
t*.
Oms.
CoCUper
zoo Gms.
Solutioa.
— 10
27.0
0
295
+ 10
315
20
33-5
25
345
30
35-5
it
60 47-5 Coa,.ILO (blue)
80 40. «; ^'
49.5
" 100 51.0 "
Solubility op Cobalt Ammonium Chlorides in Water.
(Kumakoff — J. russ. phys. chem. Gcs. 34* 629. '93; J. Chcm. Soc. 64, ii. 509, '93.)
g. Grama per 100 Grama HiO at:
ST 16.9*. 46!?.
CoCl,.sNH, 0.232 ... 1. 031
CoCV5NI^.H,0 16.12 24.87
CoC^.6NH, 4.26 ... 12.74
257
COBALT CHLOBZDS
Solubility op Cobalt Chloride in Aqueous Hydrochloric
Acid Solutions at o®.
(Engd — Ann. cbim. phys. [6] 7> 355« '89O
imUgram Mob.
per 10 cc. SoL^
KoClt.
62.4
58.52
50.8
37 25
12.85
.4.75
12 .0
25 O
HO.
O
3-7
"•45
25.2
55 o
74. 75
104 -5
139.0
Sp. Gr. of
Soltttioos.
I
I
I
I
I
I
I
I
343
328
299
248
167
150
229
323
Gxns. per 100 Gms.
Solutiop.
CoQi. HO*.
30.17 0.00
28.62 0.102
25 -39 0.321
19 -43 0738
7,15 I. 718
2.68 2.369
^♦34 3099
12.27 3-829
Gms. per xoo cc.
Sdurion.
CoCla.
40.5
38.0
33 o
24.2
8.34
308
7.79
16.24
HQ,
O
0.135
0.417
0.919
2.00
2.72
3.81
5 07
Solubility 09 Cobalt Chloride in Aqueous Alcohol
AT II. 5^
(Bfidtker^Z. phyaik. Chem. aa* 509. '97.)
10 gms. of CoClt.6HaO were added to 20 cc. of alcohol and in addition
the amounts of CoCU shown in the second column. The solutions were
shaken 2 hours, 5 cc. withdrawn, and the amotmt of dissolved CoCls
determined by evaporation and weighing.
Vol.% Gutt. CoCU GiM.pcr5cc.Solqdon
Akohol
91 -3
98.3
98.3
99-3
99-3
99.3
Added
0.0
0.0
0.0
0.0
0.194
0.400
So7
1-325
1 .134
1.068
I 045
0.899
0.829
Coat.
1. 168
1. 214
1. 181
1. 199
1.204
1.325
Vol. % Gms. Cods
Alcdiol. Added.
99
99
99
99
99
99
3
3
3
3
3
3
0.612
0.813
1.022
1.240
1.446
1.650
Gmfl. perscc.Sol.
HjO.
0.764
0.688
0.634
0.553
0.483
0.500
Coda.
1.459
1.568
1.713
1.831
1-943
2.183
ICO gms. sat. solution in alcohol (0.792 Sp. Gr.) contain 23.66 gms.
CoQ«» St). Gr. » I.OIO7. OK^nkler — J.pr.Chein.oi«M7,'64^
Solubility op Cobalt Chloride in Organic S(x.vbnts.
Sotvent.
f.
' CoOt. C0CI1.2H/).
Authority.
Acetcme
0
9. II 17.16
((
22.5
9.28 17.06
u
25
8.62
(Krug and McEIioy, 1893.)
u
18
2.75
(Naumanni 1904.)
Ethyl Acetate
14
0.08
u u
79
0.26
M
Ether, Abs.
• . •
0.021 0.291
(Bfidtker, 1897.)
Glycol
. * •
io.7(perioog.sol.)
(de Conmckp 1905.)
Acetonitrile
18
4.08
(Naunuton and Scfaier, X914O
Methyl Acetate
18
0.369*
(Namnann, 1909^
95% Formic Add
20.S
6.2
(Aichan, 19x3.)
Anhy. Hydrazine
±15
1
I
* ^ flat sol. *- a938.
(Wdih and Bxodenoo, X9XS)
COBALT CHLOBIDS 258
Solubility of Cobalt Chloride in Pyridinb.
(Pearce and Moore, 19x3.)
*• nE^JrifSi Solid 4. ^'J^& Solid 4. nS??«rS Solid
—48.2 O C|H»N 34.6 0.749 i^ 74.8 2.037 x.a
— 50.3 EutCC ... "+ X.6 37.6 0.754 •* 78.2 2.276 "
—45 0.4185 x.6 44.6 0.950 *' 79.8 2.428 **
—30 0.4205 " 47.2 1.020 •« 88 3.284 ••
— 19.6 0.4208 ** 51 i.iio « 90tr.pt. ... ••+C0CI1
— 10 0.4310 " 55 1192 " 965 7251 CoCW
o 0.4307 * 60 1.324 " 98.8 7936 **
15tr.pt. ... X.6+X.4 64.2 1.460 " 106 12.540 "
23 0.569 X.4 68 1.572 " no 14.165 "
25 0.575 " 70tr.pt... " +x.a
1.6 = CoCl,.6CiH»N. 1.4 - CoCli.4CiH6N. 1.2 -,CoCli.2C|H*N.
COBALT CITRATES- solubility in Water.
(Pickering, 19x5.)
&ns. per xoo oc. Sat. SoL
Salt. Formula. t*. ^o^ Salt
(anhydrous).
Cobalt atrate (normal) Coi[(COO.CH»)»C(OH)COO],.2H|0 10 0.08 0.267
Cobalt Hydrogen Citrate CoH[(COO.CHa)jC(OH)COO] 10 0.20 0.906
Cobalt Potassium Citrate KCo[(COO.CH2)»C(OH)COO].4HiO 10 1.05 5. 11
Cobalt Potassium Citrate K4Co[(COO.CHi)iC(OH)C(X)li 10 3.04 31
COBALT FLUORIDE CoF2.4H^.
100 gms. sat. solution in water contain 2.23 gms. of cobalt fluoride of a variety.
100 gms. sat. solution in water contain 2.32 gms. of cobalt fluoride of fi variety.
(C^ostacheacu, x9xo0
OOBALT lODATB Co(IO,),.
Solubility in Water.
(Meuaaer — Ber. 34* 3435, 'ox.)
Solid Phaae:
Co(IOi)».aHiO. CoClOth'
t\
Co(IO|)
94HsO.
' G.
M.
0
054
0.028
18
0.83
0.038
30
1.03
0.046
so
1.46
0.065
60
1.86
0.084
6S
2.17
0.098
75
• • .
...
100
. • •
• • .
G.
M.
'g.
u.
032
0.014
• « •
■ • •
0.45
0.020
I 03
0.046
0.52
0023
0.89
0.040
0.67
. . •
0.030
« • •
0.8s
• • •
0.030
• • •
• . ■
0.84
• • •
0.038
■ • •
0-7S
...
0033
1.02
0045
0.69
0.031
G a Gms. Co(IOs)t per loo gms. solution. M » Mols. Co(IOa>a
per too Mols. H2O.
OOBALT IODIDE Col,.
Solubility in Water.
(Etaxd — Compt. rend, xxa* 699. '9X; Aim. chim. phya. [7] a^ SSTt ^M^
The accuracy of these results is doubtftd.
Gms. Coll
Gms. Cola
t*.
perxoo Gmy.
Solutioiii.
Solid Phaae.
f.
periooGma.
Solution.
SoUdPhaM.
-10
55 S
CoI,.H,0 (green)
25
<57-5
CoI,.H,0 (oUve)
0
58.0
«
30
70. 0
((
10
61.5
u
40
75 0
CoI,.H30 (yello?
15
63.2
tt
50
79.0
«
20
65.2
u
80
80.0
a
«s
67
u
no
81.0
M
259
COBALT MALATK
COBALT MALATI Co(C00.CHi.CH0HC00).2Hi0.
100 cc. sat. solution in water contain 0.14 gm. Co « 0.453 S^* anhydrous salt
at 10'.
COBALT MAL0NATI8.
S(H.UBILITT OF COBALT MaLONATBS IN WaTBR.
(Lord, 1907.)
(PidLeringp 1915.)
Sdt.
Cobalt Malonate
** Ammonium Malonate
" Caesium "
" Potassium "
Fonniila. t^.
CoCHt(COO)s.2HiO 18
Co(NH4),lCHa(COO),l,.4BM) 18
CoCsi[CHa(COO)sl,.4HtO 18
CoK«(CHt(C(X))ili4HiO x8
Gnu. Aslbiy*
diousSalt
periooGms.
Sat. SoL
1-353
10.61
14.23
4.36
per 100 Gms.
SolutioQ.
OOBALT HITBATB Co(NO,),.
Solubility
(Funk — WiiB. Afah. p. t.
Gum. Mols.
CoQfO^i CoCSOuh SoUd Phjue.
per xoo
6.40 Co(NQi)i.9HiO
7-35
6.98
7.64
7 99
8.26
9.71
IN Water.
RaduusUlt 3* 430, '00.)
Gms.
^o Co(NC^
* per xoo Gms.
Sotation.
Solid FhM
-26
-20.5
— 21
— 10
— 4
O
+ 18
39-45
42.77
41.55
43.^
44-85
45.66
49 73
Co(NOfe)s^6HiO
41
55
62
70
84
91
Density of solution satttrated at z8^
55 96
62.88
61.74
62.88
64.89
68.84
77.21
1-575-
Mob.
Q>(NQw
per xoo
Mols.HsO.
12.5 Co(NQ0>4SHflO
16.7
15.8
16.7
18.2
21.7
33-3
Co(NO»)s.sHiO
SoLUBiLrnr of Cobalt Nitratb in Glycol.
(de Coninck, X905.)
100 grams saturated solution contain 80 gms. cobalt nitrate.
COBALT RUBmiUM NTTBITB RbiCo(NOi)6.HA
100 gms. H^ dissolve 0.005 Rin. of the salt. (Rosenbbtdt, x886.)
COBALT OXALATE Co(COO)i.
100 gms. 95% formic acid dissolve 0.04 gm. Co(COO)t at 19.8^ (Aacfaan, 19x3.)
COBALT SULTATK CoS04.7H^.
Solubility in Water.
f.
o
5
10
IS
20
25
30
(Mulder; Tobler, 1855; Koppd, Wetsd, 1905.)
Gms. C0SO4 per ^
xoo Gms. Der xoo ' t*.
Solution.
20.3s
21.90
23.40
24.83
26.58
28.24
29.70
Water.
25. SS
28.03
30.55
33 05
36.21
39-37
42.26
Mols.CoSO|.
per xoo
Mob.H|0
Gms.CoS04per
xoo Gms.
2
3
3
3
4
4
4
958
251
540
831
199
560
903
35
40
50
60
70
80
100
Solution.
31-40
32.81
35-56
37.65
39.66
41.18
45.35
Water.
45.80
48.85
55.2
60.4
65.7
70
83 .
Mols.CoSOb
per 100
Mols.H^.
5.31
5.664
100 gms. HsO dissolve 37.8 gms. C0SO4 at 25*
Freezing-point data (solubility, see footnote, p. i) for mixtures of C0SO4 4-
Li|S04, C0SO4 + KiSOiand C0SO4 + NaiS04'are given by
(1913)-
(Wagner, igxa)
of C0SO4 +
Calceigni and Marotta
COBALT SULFATE
260
Solubility op Mixtures op CoS04.7H,0 and Na,S04.ioH/)
IN Water.
o
5
10
20
25
30
35
40
18.5
20
25
30
35
40
18.5
20
25
30
35
40
Gmfl.
100 Gms.
ution.
(Koppd; Wetsd.)
Gms. per Mob.
100 Gms. HsO. xoo Mols.
Co.SO«.
Na^SO«.
C0SO4. Na»
16.56
7 63
21.85 10.
17
.46
9
59
^3
94 13-
17
90
II
73
25
.41 16.
17
59
16
43
26
.65 24-
17
06
15
70
2$
36 ^3'
15
94
14
93
^3
15 21.
IS
73
14
52
22
54 20.
14
87
14.
22
20.
98 20.
18.
75
IS
61
28.
61 23.
19.
30
IS
10
29.
42 23.
20
30
13
60
30
74 20.
21
67
12.
05
32
70 18.
22
76
10.
43
34
06 15.
24
OS
9
.16
35
01 13.
16
87
16.
97
25-
SO 25.
15
41
18.
12
23
18 27.
10
63
23
26
i6.
07 35-
6.
01
28.
67
9
20 43-
4
56
32
14
7-
19 50.
4
72
31
78
7
45 50.
07
IS
67
91
32
61
8s
OS
82
01
58
17
61
72
6S
26
17
74
79
10
SSo.
C0SO4.
^•54
2.77
2.94
3 09
2.95
2.70
2.62
2.46
3-3^
3 41
3 56
3-79
3-95
4.81
2-. 96
2.69
1.86
1. 07
0.835
0.864
NaiS04.
1.27
1.67
2. II
315
2.97
2.74
2.64
2-53
3 02
2.92
2.61
30
98
74
25
45
4.46
5 54
6.44
6.34
3
3
Solid Phase.
C0SO4.7HJO +
NaaS04.ioH^
CoNat(S04)s.4H^
K
U
CoNai(S04)t.4HiO
+ CoS04.7HiO
u
«(
M
it
CoNaflCSOJt^HiO
+Na^SO4.ioH40
««
CoNat(S04)t.4H«0
+NaaS04
M
Solubility op Cobalt Sulphate in Metkyl and Ethyl Alcohol
AND IN Glycol.
Sotveot.
Gma.
to.
per xoo Gms.
Sdvent.
K
OuSCl'VU.
C0SO4.
CoS04.7H«C
.
Methyl Alcohol (abs.)
3 ••
42.8
(deBniyft— Z. phyaik.Ch. zo^ 784, 'psO
tl it
u tt
(93.5%)
(50%)
Ethyl Alcohol (abs.)
15 ...
18 I .04
3 •••
3 • •
3 •••
50.9
54.5
^3-3
1.8
2.5
•i
M
M
i4
M
Glycol
. .(per 100 gms.
solution) 3.1
(deConmck—
3Sg. '05.)
' Boll. acad. roy . Bdgique,
COBALT SX7LFIDK CoS.
One liter water dissolves 0.00379 gm. CoS at 18^ (electrolytic conductivity
method, assuming complete dissociation and hydrolysis). (Wdgd, 1906.)
36l
COCAIME
COCAINK CnHaNOi.
SOLUBILITT IN SEVERAL SOLVENTS.
Gms. Cn%NOi
per xoo Gms.
Sdvent.
f.
Autbonty.
Solvent.
Water
20
0.028
(ZaUu, 1910.)
«
±20
0.140
(Baroni and Bariinetti. zQzzO
l€
as
0.17
(U. S. PO
a
80
0.38
«
3 0ms. H<BOk in Ag. 50% Glycerol
±20
8
(Buoni and BarBnetti, 191ZO
Alcohol (92.5 Wt %)
25
20
(U. S. P.)
Ether
25
26.3
i(
((
18-22
ZI.6
(Mailer, 19013.)
Ether sat. with U/)
z8-22
34
u
Water sat. with Ether
18-22
0.254
M
Aniline
20
76
(Scfaokz, 191a.)
Carbon Tetrachloride
20
31 -94
(Gori. 1913.)
Chloroform
18-22
100 -f
(Mailer, 1909.)
Benzene
18-22
100
II
Ethyl Acetate
18-22
59
<•
Petroleum Ether
18-22
2.37
u
Pyridine
20-25
80+
(Dehn, 1917; Scbdts, 19x9.)
Piperidine
20
56
(Scholtz, 191a.)
nipthyl^LfniTM
20
36
4. 34*
u
SeaeimeOil
20
(Zalai, 19x0.)
Olive Oil
25
8.3
(U. S. P.)
Oil of Turpentine
25
7.1
u
• Per 100 cc.
COCAINK HTDROCHLOBIDS
CnHa
NO4.HC!.
100 gms. HiO 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 6o^ (U. S. P.)
100 gms. chloroform dissolve 5.4 gms. salt at 25**. (U. S. P.)
100 gms. glycerol dissolve 25 gnis. salt at 15^. (B.P.)
COCAINS PEBCHLORATE C17HS1NO4.HCIO4.
100 gms. HsO (containing 8% free HCIO4} dissolve 0.26 gm. perchlorate at 6^.
(Hofmann, Roth, Hdbold and Metzler, 19x0}
CODEINE Ci8HsiN0|.H,0.
CODEINE PHOSPHATE Ci8HtiNOs.H,P04.2HiO.
CODEINE SULFATE (CisHnNOs)i.H,S04.5H,0.
Solubility of Each Separately in Several Solvents.
Gms. per zoo Gms. Solvent.
Sdvent.
Water
Alcohol (92.3 Wt %)
« (I
Methyl Alcohol
Chloroform
Carbon Tetrachloride
Ether
Benzene
Trichlorethylene
3 Gms. H«B(^ per 100 cc.
aq. 50% Glycerol ord. t.
f.
Codeine.
C. Phos-
phate.
C. '
Sulfate.
Authority.
25
0.80-1.7
44.9
3-3
(U. S. P.; Baroni and Barlinetto,
20
0.84
• • •
• • ■
(Zalai. 1910.) [19x1.)
80
1.70
227
16
(U. S. P.)
25
637
0.383
O.I
(Schaeffer, 1913; U. S. P.)
60
108.7
1.03
0.27
(U. S. P.)
25
62.8
• • •
0.56
(Schaeffer, X9Z3.)
25
133-151
0.015
0.007 (Schaeffer, U. S. P.)
20
2.94-1.33
• • •
• • •
((jori. 19x3; Beilfltein, SoppL)
25
8
0.075
• • • •
(U. S. P.)
25
II. 4
• • •
Insol.
(Schaeffer, 19x3.)
15
12
• • •
• ■ •
(Wester and Bruins, 19x4.)
4 ... ... (Baroni and Barlinetto, I9xx0
100 gms. trichlorethylene dissolve 0.014 gm. codeine hydrochloride at 15^.
(Wester and Bruins, 19x4.)
Data for the solubility of codeine and codeine sulfate in mixtures of alcohote,
benzene and chloroform are given by Schae£Fer (1913).
COLCHICINI
26a
COLCHICINI
Solveiit.
Water
«
Ether
«
C«H,NO..
Solubility in Several Sch^vemts.
(MQller. 1903; U. S. P.)
Cms.
CalWiO,
per 100 Gms.
Solvent.
9.6
45
13 -7*
r.
Solvent.
sat. with HiO
18-22
80
82
18-22
as
18-22
0.13
0.64
0.18
Water sat. with Ether
Benzene
Benzene
Chloroform
Carbon Tetrachloride
Ethyl Acetate
Petroleum Ether
r.
x8-22
18-22
25
18-22
18-22
18-22
x8-22
Gm.
CsHaNOb
per 100 Gms.
Solvent
12.05
0.94
LIS
100+
0.12
1.34
0.06
COLCUiClMS SALTS.
Name.
Fonmiku
r.
Colchicine lodohydrate CttHiiNOt.HI Water
Iso Colcnidne lodohydrate " "
Colchicine Silicotungstate l^^SSSJgP'lAil.xroHa'x's
30
30
Gms. Salt
per Liter
Sat. Sol.
0.84
3.86
0.083
0.007
Anthflrity.
(Pfiiml, Z911O
M
1913^
COLUDINS (24.6 Trimethyl Pyridine) C»HtN(CHt)s.
Solubility in Water.
(Rothmund, 1898.)
Gms. CoOidine per 100 Gms.
r.
Aq. Layer. Collidine Layer.
5.7crit. t. 17.20
10
20
30
40
60
7.82
3 42
2.51
1-93
1.76
41.66
54.92
62.80
70.03
80.19
r.
80
100
120
140
160
180
Gms. Collidine per 100 Gm.
Aq. Layer. Collidine Layer.
1-73
1.78
1.82
2.19
2.93
3 67
86.12
88.07
88.98
89.10
87.2
COLUDINI (1.3.5 Trimethyl Pyridine) CiHtN(CHt)s.
Distribution between Water and Toluene.
(Hantzach and Vagt, 190Z.)
G. Mols. Collidine per Liter.
G. Mols. Collidine per Liter.
**• H,0 Uycr.
Toluene
Layer.
^ Dist. Coef.
HiOUyer
0 0.003s
0.0580
0.0603
50 0.0017
10 0.0026
0.0587
0.0443
70 0.0015
20 0.0022
0.0588
0.0374
90 0.0013
30 0.0020
0.0594
0.0337
CONGO RED
[C6H4.N : N.CioH,(NHi)SO,Na],.
Toluene
Layer.
0.0596
0.0597
0.0598
Dist. Coef.
0.0285
0.0251
0.0218
(Dehn, 19x7.)
K
<l
100 gms. H»0 dissolve 11.6 gms. congo red at 20®-25*.
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) CsHkN.
100 gms. H2O dissolve 1.83 gms. coniine at 20^.
COPPER ACETATE Cu(C,H«0,),H,0.
100 jnns. glycerol (du » 1.256 » 96%) dissolve 10 gms. copper acetate at
I5*-l6^ (Osiendowski. 1907O
(Zalai. Z9Z0.)
263 COPPER ACSTATI
SOLUBILITT OF ANHYDROUS COPPBR ACBTATB IN PYRIDINE.
(Mathews and Benger, 1914.)
Giiis.Cu(C|H^O^ Gms.Cu(qHa0^s
r.
per 100 Gibs
SaLSoL
SoUd Phase.
t*.
per 100 Gma.
Sat. Sol.
SoUdPhaae.
~ii.6
0.37
CuCCAQOmCJHiN
45-2
4.17
Cu(CHA)s.4QH.N
+ i
0.6
i<
34-8
3-75
Cu(CAOk)t.CAN
13
1.03
<(
SS-7
4.13
M
26.45
1. 61
■i
64 -3
4.48
M
37-4
2.83
u
76.2
4.83
M
41.9
312
M
83 -3
S-40
«
43-3
3-39
«
95-4
6.31
M
Transition point » 44.7^.
COPPER ^BROMIDE (ous) CuiBr,.
Solubility op Cuprous Bromide in Aqueous Solutions of Potassium
Bromide at i8*-20®.
(Bodlllnder and Storbeck, 1903.)
Millunols per Liter. Grains per Liter.
KBr. Total Cu. Total Br. Cu (ic). Cu (ous). KBr. ToUl Cu. Cu (ic). Cu (ous).
o 0-3157 0.4320 0.2096 0.1061 o 0.0201 0.0133 0.0067
25 0.II9 ... 0.012 0.107 2.98 0.0076 0.0007 0.0068
40 0.200
60 0.310
80 0.423
100 0.584
120 0.693
500 8.719
0.013 0.187 4.76 0.0127 0.0007 O.OII9
0.025 0.285 7.15 0.0197 0.0015 O.O181
0.012 O.41I 9.53 0.0266 0.0007 0.0261
0.584 II. 91 0.0371 ... 0.0371
0.693 14- 29 0.0441 ... 0.0441
8.719 59.55 0.5540 ... 0.5540
100 gms. acetonitrile dissolve 3.86 gms. CuiBri at iS**. * (Naumann and Schier, 1914.)
Freezing-point lowering data for mixture of CuBr + KBr are given by de
Cesaris, 191 1.
COPPER BROMIDE (ic) CuBrt.
100 gms. acetonitrile dissolve 2^.43 gms. CuBri at 18**. (Naumann and Schier, 1914.)
ICO gms. 95% formic acid dissolve 0.16 gm. CuBri at 2i^ (Aschan, i9z3-)
COPPER CARBONATE Basic.
Solubility in Aqueous COi Solutions at 30®.
(Free, 1908.)
Aq. 0.5 n NaaCOi and 0.5 n CuSOi were mixed and the precipitate washed and
suspendc^d in HsO containing COi 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 ot the constituents was found to be iCuO:
0.51^ COi: 0.61 H2O. For the solubility determinations, about 2 gms. of the
preapitate were suspended in 600 cc. of HsO and COt passed in to the desired
concentration. The mixture was shaken frequently for 3 days. The total COi
in the sat. solution was determined and the free COi calc. by difference, assuming
that the amount combined to the Cu was in the molecular ratio 2CuO:iCO|.
Parts per Million. Parts per Million.
Free C(V Metallic Co.
FreeCCH-
Metallic Cu.
o=puieHiO i-s
859
28
IS7 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 C0| at x + atmosphere.
Results practically identical with the above were obtained for a NaCl solu-
tion contaming 100 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 CABBONATK
264
SoUd Phase.
Solubility of Mixtures of Copper Carbonate and Potassium
Carbonate in Water at 25**.
(Wood and Jones, 1907-^.)
100 gms. HsO dissolve 3.15 gms. CuCOi + 105 nns. KiCOi at 25^ when the
solid phase in contact with the solution is CuCOi.KsCOi + KiCOi.
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, CuCO|.KsCOi:
Gms. per 100 Gms. HfO.
&,C0|. CuCO,'.
IDS 3. IS K«CQrfCuCQ8.KaCQ|
100 3 . 20 CuCQ8.K2COi
90 3 40
8s 3.60
The triple point for double salt + CuCQi could not be determined sinoe
CuCOs is not capable of existing alone and decomposes into COi + Cu(OH)i.
COPPER CHLORATE (ic) Cu(C10s),.4H,0.
Solubility in Water.
(Meusser, 1962.)
r.
—12
-31
—21
Gms.
Mols.-
CuCClO^t CuCClOOt Solid Phase,
per 100 Gms. per 100 MotB.
Sohitions. H«0.
30.53 3.43 Ice
54.59 9.39 Cu(aQi),.4Hd0
57- 12 10.41
11.02
Gms. Mols.
t*. CuCClO^fl Cii(aCW)| Soli
per zoo Gms. per 100 McMs. ^
Solid Phase.
.<
Solutioiis
18 62.17
45 66.17
59.6 69.42
71 76.9
+ 0.8 58.51
Density of solution saturated at 18® » 1.695.
COPPER CHLORIDE (ic) CuCU.2HsO.
Solubility 'in Water.
(Reicher and Deventer,' 1890; se6 also Etaid, X894O
12.84 CttCao^fAO
15.28
17-73
25.57 -^
Gms. CuCU
t*. per zoo Gms.
Solution.
f.
Gm.1. Cudt
per xoo Gms.
Solution.
r.
Cms. CaCW
per xooGiitt.
Solution.
—40 Eiitec 36.3
20
43. S
50
46.6s
0 41.4
2S
44
60
47.7
10 42.4s
30
44-55
80
49.8
17 43-o6
40
45-6
100
51-9
Density of solution saturated at o® = 1.5 11, at 17.5® = 1.579.
100 gms. sat. solution in water contain 43.95 gms. CuCli at 30% solid phase*
CuCli.2HtO. (Sdireiiiemakers, z^ia)
COPPER CHLORIDE (ous) CuCl.
100 gms. HsO dissolve 1.52 gms. CuCl at 25^ (Nom, x9xa.)
Solubility of Cuprous Chloride in Aqueous Solutions op Hydrochloric
Acid Containing CuClj at 25®.
(Poma, 1909, 1910.)
Results for 2 n HCl.
Mols. per liter.
Results for i n HCl.
Mols. per Liter.
6aO
Solid
mSI CuCW+CuCL Phase.
O 0.0862 CuQ
0.1 0.2017 •*
0.2 0.3256
0.4 0.5707
0.5 0.6924
«
«
CuCU
Added.
0.094
0.188
0235
0.282
SoUd
CuOa+CuCL Phwe-
0.2365 CuQ
0.3528 "
0.4766 ••
0.538s "
0.6038 -
Results for 4 n HQ.
Mols. lyr Liter. ^^
AdS. Cua,+Cua. Ph«.
o 0.7704 Caa
0.095 0.9044 "
0.189 1.0370 "
0.379 1.3040 •
0.473 1.4380 «
365 COPPER CHLORIDK
SoLUBiLiTT OP Cuprous Chloride in Aqueous Solutions op Hydro-
chloric Acid.
(Engel — Ilrid.i6\ z7t 37'» '^\ Compt. xend. lax. 529* '95.)
BliOignm Mob
.j)er xocc. Sd.
Sp. Gr. of
Solutioos.
Cms. prr xoo cc. Sol.
Gma. per xoo Gms. Sol.
iCuaQa.
HQ.
Curf3i.
hq:
CiiiOa.
ho:
ResalUat<
)•.
0-47S
8.97s
1.05
0.471
0.327
0.448
0.312
i-S
I7-S
1. 049
1.486
0.638
1. 418
0.608
2.9
26.0
1.065
2.872
0.948
2.697
0.932
45
34 S
1.080
4.457
1-257
4.127
1. 164
8.2s
47.8
1135
8.172
1-743
7.199
1-535
T^S'S
68.S
1. 261
15-7
2.497
12.46
1.980
33 0
104.0
1-345
32.68
3.827
24.30
2.845
Reaoksat
li'-ifi'.
7-4
54.4
1. 19
7-33
1.983
6.159
Z.666
10.8
68.9
1.27
10.69
2.5x1
8.422
1.977
12.8
75 0
1.29
12.68
«-734
9.826
2. 119
16 0
92.0
1.38
15.84
3-346
11.48
2.424
Solubility op Cupric Chloride
« •
IN Aqueous Solutions op Hydro-
chloric
Acid AT o^
(Engel ~- Ann. cfaim. iihys. [6]
17. 351. '89.)
MOSgFam Mob
. per TO cc. Sol.
Hd.
Sp Gr. of
Solutions.
Cms. per
100 cc. SoL
Gma. per x
CuOs.
00 Gms. Sol.
^uQa.
duOa.
Ha:
hcl^
91 -75
0
1.49
61.70
0.0
41.41
0.0
86.8
4.5
1-475
58.37
1.64
39-58
I. II
83.2
7.8
1.458
55-95
2.84
3837
1-95
79-35
10.5
1-435
53-37
3 83
37-19
2.67
68.4
20.25
1.389
46.01
7-38
33'^^
5 31
50.0
37-5
1-319
33-62
13-67
25-50
10.37
22.8
70.25
1. 231
15-33
25.61
12.46
20.80
^3-5
102.5
1.288
15-81
37 36
12.27
29.00
26.7
128.0
I 323
17.96
29.0
46.66
Sat. HCl
13 57
35-26
Copper Chloride, Ammonium Chloride Mixtures m Aqueous
Solution at 30®.
(Meerbiug — Z. anofg. Chem. 45* 3, '05O
Grams per zoo
Gnuns per xoo
Gms. Sat.
Soludon.
Gms.
Solid Phase.
SoldPlUM.
'cua..
NH4a.'
CuOa.
NHrfX
0
29-5
• • •
• • •
nh^
1.9
28.6
6.0
48.3
NHiQ + Caaa.sNH«CUH,0
3.6
25 -9
37 0
34-9
Coab.sNHda.sH«0
10.5
16.5
21.7
33 1
M
19.9
9.4
28.5
18.4
«
29.4
4.9
35-1
IS -3
M
41.4
2.Z
43.1
13-3
«
43-2
2.0
51 -9
6.6
GiiCh.sNHdCl.sH^+Caat^H^
43-9
0
» • .
•
CaCls.aHsO
Additional determinations for the ammonia end of this system at 25^ are
given by Foote, 1912.
COPPER CHLOBIDK 266
COPPIR AMMONIUM CHLORIDE CuCIs.2NH«a.2HA
Solubility IN Watbs*
(Heerbuig, 1905.)
Gm.
«• CuOf-sNIIia
* * per 100 Gms.
Solution.
Solid Phue.
r.
Gms.
cuafl.3NH«a
per 100 Gmi.
Sdution. J
Solid Phase.
10.5 3.87
Ice
30
27.70
Caat.aNH|CLaH^
10.8 20.12
4
40
30.47
M
II 20.3
Ioe+Cuat.aNHia.aH^
50
33.24
«
ID 20.46
CttCV^NHiCLaH^
60
36.13
«
0 22.02
12 24.26
M
M
70
80
39.35
43.36
M
•
1
20 25.9s
M
SoLUBiLiTT OP Cuprous Chloride in Aqubous Solutions op Cupric
SVLFATB AT ABOUT 20*.
(Bodliader and Stocbeck, 1902.)
MilHmobper]
Liter.
Grains per liter.
'CuSO«.
0
0.987
1.975
2.962
4.937
Total Cu. Total CL
2.880 " 5.312
3.602 4.908
4.553 4687
5.193 4.256
7.276 4.329
Cu (ic).
2.258
3 145
4. 131
4.625
6.546
Cu (ous).
0.622
0.457
0.422
0.509
0.730
CuSQi.
0
0.158
0.315
0.473
0.788
Total Cu. Total O.
0.183*0.188
0.229 0.174
0.290 0.166
0.330 0.151
0.463 0.154
Cu (ic).
0.143
0.200
0.263
0.292
0.416
Ctt(ous).
' 0.040'
0.029
0.027
0.032
0.046
Solubility of Cuprous Chloride in Aqueous Solutions op
Potassium Chloride at about 20^
llillimols per
Liter.
(kuBS per liter.
' Ka
Total (X
Total a
Cu Gc).
Cu (ous).^ ^ KCL
Total Cu. Total CL
Ctt (ic).
Cu (ous).
0
2.851
5.416
2.222
0.629
0
O.181
0.193
O.141
0.040
a.S
; 1.955
6.015
1. 421
0.534
0.186
0.124
0.213
0.090
0.034
5
Z.522
7.52s
1.008
0.514
0.373
0.097
0.267
0.069
0.033
zo
1.236
"735
0.475
0.761
0.746
0.079
0.416
0.030
0.048
20
1.446
21. 356
0.324
1. 122
1.492
0.092
0.7S9
0.021
0.071
50
2.41X
notdet.
0.1088
2.302
3-730
O.IS3
notdet.
0.007
0.146
100
4.702
«
0
4.702
7.460
0.299
(f
0
0.299
200
9.48s
«
0
9.485
14.920
0.603
tt
0
0.603
1000
97
u
0
97
74.60
6.170
li
0
6.170
2000
384
l€
0
384
149.2
24.42
f(
0
24.420
The results in the 3d, 7th, 8th and last line of this table are at I6^
Solubility op Copper Chloride in Aqueous Solutions of Sodium
Chloride.
(Hunt, 1870.)
Gms. CuClt per xoo cc. Solution of:
r.
Sat. NaCl.
15% NaQ.
S% Nad:
II
8.9
3.6
• • •
40
II. 9
6
I.I
90
16.9
10.3
2.6
267
COPPER CHLORIDE
Solubility of Cuprous Chloridb in Aqueous Sch^utions of Fe&rous
Chloride at 21.5*^ and Vice Versa.
(Ejcmann and Noas, 191 2.)
In order to ascertain the composition of the solid phase, the experiment was
made by mixing together weighed amounts of HiO, CuCl and FeCli 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 di£ference.
Cms. per xoo Cms. H|0.
Fed..
CuCL
0
1-53
6.02
1-33
11.62
1.80
16.30
3"
26.30
7.12
2935
8.06
33 12
956
Solid FhaM.
CuCl
Gms. per zoo Gms. H4O.
Feci,.
CuCL '
OQua r naae.
43-75
12.42
CuCl
54
17.04
(t
66.40
21.6
((
73.20
23.20
" +FeCl,.4HjO
71.90
21.65
FeCl«.4H|0
69.30
II. 9
it
65.10
0
tt
Solubility of Cuprous Chloride in Aqueous Solutions of Sodium
Chloride at 26.5^ and Vice Versa.
(Kicmaim and Noas, 191a.)
(See remarks above.)
Gmt. per xoo Gms. H|0.
Naa.
CuQ.
soaa row
0
10.8
1-55
3.15
CuCl
10.7
27
36.48
7.30
40.60
49.10
(C
Gms. per xoo Gms. H^.
Naa.
CuCL '
SdBd Phase.
44.14
57.21
Cua
55- 10
44.10
NaCl
56.80
41.70
(t
50.90
18.70
«
Solubility of Cuprous Chloride in Aqueous Solutions of Potassium
Chloride at 22^ and Vice Versa.
(BrSnsted, 19x2.)
Gms. per xoo Gms.
Sat.SoL
SolM
Phase.
Gms. per
Sat.
xoo Gms.
Sol.
Solid
Phase.
Gms. per i
Sat.
[ooGms.
Sol.
Solid
Phase.
KQ. Cua.
. rcL
Cua.
Ka.
CuCl.
3.87 O.II5
CuQ
21.64
13-32
CuQ
24.04
4.53
cua.3Kci
6.56 0.405
8.24 0.861
ff
w
23-84
25-24
17.23
21.47
M
M
25-03
26.28
3-14
2.20
M
11.33 2.19
M
23-87
15-48
Cua.aKa
27.06
1.60
M
15-30 4. So
»
23-57
13-99
u
26.68
I. 21
Ea
17.47 7.19
M
23.50
"39
M
26.32
0.58
ft
ao.31 10.21
«
23.49
7.35
M
25.68
0
.«
COPPKB CHLORIDE
268
Solubility of Cupric Chloridb in Aqubous Solutions op Mbrcuuc
Chloride at 35° and Vice Versa.
(Schrdnemftken and Thomis, 1912.)
- ,. . n, Gms. per 100 Gms. Sat. Sol.
GnM.'per loo'Gms. Sat. SoL
HgCW
CuCl,.
ouua x-uaac
HcO,.
CuC^
0
21.03
44-47
33-5
CuClt.2H|0
52.54
52.81
18.46
18.06
37.30
26.07
tt
51 03
14-73
44-47
50.47
52.44
23-31
21.50
19.40
It
" +Hga,
HgCl,
49.50
23.87
8.51
5-94
2.64
0
Solid Phase.
HgCl,
Solubility op Copper Chloride and Potassium Chloride Doublb
Salts and Mixtures in Water.
(Meycrikoffer — Z. phyrik. Chem. s xoa* '90O
Q per I Gram Solution.
Mok. per 100 Mob. HaO.
%:
'Preaent aa
CuQs.
Preaent aa'
KCL
CaQs.
KQ.
aoaa
Phaae.
39-4
0.120
0.107
5-56
9-93
Caas.aKa.aHsO + KQ
49-9
0.129
o.ns
6-39
II. 4
M
60.4
0.142
0.125
7.71
13.6
••
79.1
0.168
0.142
II. I
18.8
M
90 s
0.188
0.154
14.9
24.4
M
93-7
0.194
0.156
16.2
26.0
CuasJsia+Ka
98.8
0.197
0.162
17-5
28.7
It
0
0.214
0.021
9.84
1.94
Cttas.aKa.aHsO + Caas.aHs<
39-6
0.232
0.049
12.9
S-44
M
50.1
0.233
0059
ni
6.90
M
52.9
0.241
0.062
14.8
1-^3
«•
60.2
0.246
0.066
15.8
8.49
CuasXa + Caas.aHsO
72.6
0.2SS
0.063
16.8
8-35
M
64.2
• • •
...
14.9
II. 6
Cttas.aKa.3Hs0 + Cudsxa
72.5
* • •
• • •
14.8
15-0
CaCIsXa
Solubility of Cupric Chloride in Aqueous Solutions of Sodium
Chloride at 30° and Vice Versa.
(Srhrrinrmakera and de Baat, 190S-09.)
Gma. per 100 Gms. Sat. Sol.
Naa.
CuQ,.
ooua ruase.
0
43-95
CuCl,.2HaO
3.10
4.28
41.14
41.06
6.41
10.25
12.02
39-40
36.86
32.38
it
" +NaCl
NaCl
Gms. per zoo Gms. Sat. Sol.
NaCl.
Cud..'
12.25
32.40
13.54
28.64
15-40
23-72
18.44
16.98
20.61
11.03
26.47
0
Solid Phase.
NaQ
26$
COOPPER CHLORIDE
Solubility of Cupmc Chlohi6^ nl Aqueous Alcohol at^ils".
(BOdtker, 1897.)
10 gms. of CuClisHsO and the indicated amounts of CuClt were added to
20 cc. portions of alcohol. The solutions shaken two hours Jand 5 cc. portions
withdrawn.
Vol. % Gms. Cud, Cms. pCT sec. Solution.' Vol. %
Alcohol. Added. ' H|0. CuC1«. ' Alcohol.
89.3 o 0.794 1. 137 99-3
92.3 o 0.648 1.090 99.3
96.3 o 0.478 1. 116 99.3
99.3 o 0.369 1.208 99.3
Gms. CuCl» Gms. per s cc. Solution.
Added. ^ ^ h^. , CuCl».
0.223 0.330 1.29s
0.887 0.247 1-639
1.540 O.I9I 2.086
1.957 0.164 2.400
Solubilitt op Cupric Chloridb in Sbvbral Solvents.
(Etud — Ann. chim. phys. [7] a* 564, '94; de Bruyn — Z. phyaik. Chem. 10^ 783* '93* de Coniiick -*
Compt.rend. 13 x* 59, '00; St. von Laszcxynski — Ber. a7f ^aSs, '94.)
Solvent.
Grams CuQa per xoo Grams Sat. Solution at:
XT
36
32
29
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Iso Propyl Alcohol
n Butyl Alcohol
AUyl Alcohol
Ethyl Formate
Ethyl Acetate
Acetone (abs.)
Acetone (80%)
Ether
* (Cuaa.A Aq.)
if'
40.5 (deB.) 36.5
35.0 (deB.) 35.7
30s
IS
23
10
40'.
37 o
39 o
30s
16.0
16.0
So**
S.S6* 8.92t
IS -3
23.0
9.0 8.0
3-0 2.5
2.88(18^) ...
18. 9$
o.ii
t (a3*^ Cuas.^ Aq.)
30
16
o
S
3 (72")
40 (56^)
0.043 (ii"^)
t (Cnaa.a Aq.)
For the solubility of cupric chloride in mixtures of a number of
organic solvents, see de Coninck.
Sdvent
Acetonitrile
Ethyl Acetate
Methyl Acetate
f.
18
18
18
Gms.
CuCli per
xoo Gms.
Sat. Sol.
1. 57
0.4
0-S5
Sp. Gr.
Sat. Sol.
Authority.
(Naumann and Schier, i9X4«)
0 . 9055 (Naumann, 1904.)
0 . 939 (Naumann, X909.)
Anhydrous Hydrazine Ord. temp. 5 (decomp.) . . . (Welsh and Brodexaon, X9i5<)
SOLUBILrrY OF Cuprous CHLORmS in AcETONITRILB. (Naumann and Schier, X9X4O
100 gms. acetonitrile of boiling point 81.6*^ dissolve 13.33 gms. CuCl at i8^.
Solubility of Cupric Chloride in Pyridine.
: (Mathews and.Spero, 19x7.)
Gms.
• « «• *
w ^ *
w
Gms.
r.
CuCUper
xoo Gms.
Solid Phase.
r
CuCUper
xoo Gms.
Solid Phase.
-
Sat. Sol.
Sat. Sol.
-17-3
0.140
CuC1^6QH,N
45
0.422
CuC]|.2QH,N
— 12. 1
0195
M
53
0.493
fi
— 10
0.29s
** (unstable)
60
0.565
" (unstable)
- 8.9 tr.
pt.
0.270
« +CuCl,.aC|H,N
62
0.616
M «
+ 2
0.275
CuOt-sCsBcN
58 <
tr.
pt.
...
" +aCttCl,.3r<HiN
10
0.293
«
63
0.543
SCUCI1.3CAN
25
0.348
«
75
0.631
M
35
0.382
M
95
^
0.917
«
GOPPBB CHLOBIDK 270
Distribution of Cupric Chloride between aq. HQ and Ether
When I gm. of copper as chloride is dissolved in 100 cc. of 10% HCl and shaken
with 100 cc. of ether, 0.05% of the metal enters the ethereal layer. (Mylius, 1911.)
COPPER Ammonium CHLORIDE CuCIlNH^CI.
Solubility in Absolute Alcohol at 25*^. (Foote and Waiden, 1911.)
Gms. per loo Gms. Sat. Sol. ^ ,.,«,.
OiO;. " NH:a: Sobd phase.
4.7 not det. NH4CI+ CUCI2.NH4CI
6.4S " CUCI2.NH4CI
12.90 "
34.7 " " +CUCI2.C2H6OH
COPPER Potassium CHLORIDE CuCls.KCL
Solubility in Absolute Alcohol and jn Acetone at 25®. (Foote and Waldea, 191 1)
In Absolute Alcohol. In Acetone.
Gms. per looGms. Sat. Sol. Cms. per xooGms. Sat. Sol.
^ » Solid Phase. Solid Pluae.
. CuCl,. KCl. oonaruMc. CuCl,. KCT aoua rnase.
1.40 0.28 Kci+cuci,.Ka 0.34 0.38 Ka+cuci,.Ka
2.15 not. det. cuCi,.Ka 0.48 not det. CuOt-Kci
5.25 " " 1.50 "
30.16 " " 2.06 "
34.45 0.21 " +cua,.CHi0H 2.40 0.27 « +cuci,.c.ao
33.97 O CuCl«.CHtOH
Preezing-point data (solubility, see footnote, p. i) are given for the following
mixtures of cuprous chloride and other chlorides.
CuCl -\- CuCli (Sandonnini, 191a (a)).
** -|- FeCla (Hermann, 191 1.)
1; + PbCl,
-{• LiCl (Sandonnini, 19x1, 1914; Koneng, 1914.)
-{• RbCl (Sandonnini, 1914; Sandonnini and Aureggi, 19x9.)
4" AgCl (Sandonnini, 19x1, 19x4; Poma and Gabbi, X91X, 19x9.)
-f- KCl (Sandonnim,i9xi,x9X4; Korreog, 19x4; Sadcur, 19x3; Poma and Gabbi, 191 x, 191 a.)
-f- NaCl (Sandoimini, x9ix, X9X4; Korreng, 1914; Sackur, 19x3; de Cesari, 19x1.)
-f- TlCl (Sandonnini, x9xx, X9X4.)
+ SnCU (Hennann, i9n.)
" +ZnCl,
Freezing-point lowering data for mixtures of CuCl + CutO and CuCl + CuiS
are given by Truthe, 191 2.
COPPER Potassium CITRATE CuK4[(COOCHO,C(OH)C001t.
100 cc. sat. solution in HsO contain 43.3 gms. of the salt at 10^. (Pickering, 1915.)
COPPER CYANIDE (ous) Cu,(CN)s.
Freezing-point data for Cui(CN), -f- KCN and Cut(CN)2 + NaCN ar« given
by Truthe (1912).
COPPER HYDROXIDE (ic) Cu(OH)t.
Solubility in Aqueous Solutions of Ammonia at i8*. (Dawaon, 1909.)
Mob. NH« per Gm. Atoms Cu per Mols. NHi per Gm. Atoms Cu per
Liter. Liter. Liter. ^ Liter.
0.2 0.00054 3 0.0548
0.5 0.0033 4 0.0784
I 0.0109 5 O.IO4I
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, 19104.
Data showing the effect of increasing amounts of (NHOtSOi, Ba(OH)s, NaOH
and of NasSO« upon the solubility of cupric hydroxide in aqueous ammonia
solution at i8^ are given by Dawson, 1909 a.
371
COPPER lODATI
COPPER lODATE (ic) Cu(IQ8)sHiO.
One liter sat. aqueous solution contains 1.36 gms. Cu(IOs)s at 25^, determined
by measurement of single potential differences against a o.i n calomel electrode.
(Spcnoer, 19x5.)
COPPER IODIDE (ic) Cult.
One liter sat. aqueous solution contains 11.07 gms. Cult at 20^.
(Fedotieff, 1911-19.)
COPPER IODIDE (ous) Cuslt.
Solubility of Cuprous Iodide in Aqueous Solutions of Ammonium
Bromide and of Potassium Bromide.
(Kohn, 1909; Kohn, and KleiB, 191 a.)
Results for Aq. NH4Br at 20''.
NonoAli^ Gms. Cuilt
NILBr per xooo cc t*.
SoL Sat. Sol.
2 1.9068 19.5
3 3 6540 24
4 6.0588 19. s
Results for Aq. KBr 'Solutions.
Norattdity Gms. CvA Normali^ Gms. Cutlfl
t*. of KBr per xooo Gms.
SoL Sat. SoL
23 3 3 595
22 4 7.126
22 4 6.977
of KBr
SoL
2
2
3
per 1000 oc.
Sat. SoL
1.467
1.558
3.409
Solubility of Cuprous Iodide in Aqueous Solutions of Iodine at 20^
AND Vice Versa. (Ftdotidr. x9x»-zi.)
Cms, pear Liter. Solid
^^ ' L ^Ph*»e.
0.285 0.5848 CttI
0.482 1.3053
0.583 1.9218
0.678 2.5573
0.756 3.2042
0.844 3-9539
0.898 4.4359
Gms. per Liter.
«(
ti
ii
u
u
tt
Cu.
0.964
1.032
1.090
1. 112
1.232
1.040
0.898
I.
Solid
Phase.
Gms. per Liter.
«<
ti
II
5.0854 Cul
5.6854
6.2816
6 . 5301
7.6529
6.4440
5.5941
" +1
I at
.0
Cu.
0.748
0.606
0.448
0.300
0.159
Solid
Phue.
I.
4.7112
3.8562
2.9493
2.0689
1 . 2304 ••
5.4609 Cttl+I
M
«
0^=0.925
" at 40** =1.658 11.3658
Iodine determined by thiosulfate titra-
^ Constant agitation and temperature,
tion; copper, electrolyticEdly.
Additional data for the solubilitv of cuprous iodide in aqueous solutions of
iodine in presence of acids and salts at 25°, are p^iven by Bray and MacKay
(19 10). 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 ofcupric iodide and tri-iodide.
100 gms. acetonitrile dissolve 3.52 gms. CusIs at 18^. (Naumami and Schier. 19x4.)
Freezing-point lowering data for mixtures of Cul + Agl are given by Quercigh, '14.
COPPEB NITItATE (ic) Cu(NO,),.
Solubility in Water.
(Fank, 1900.)
Gms.
Mols.
Gms. Mols.
*. Cu(NOi),
• periooGms.
Cu(N0,), s^j pi^ ^
per XOO ^~"" Mruaac. m
Mols. HsO.
CuCNO), Cii(NO0i Solid Phase,
per 100 Gms. per 100 *— «*«
Solution.
Solution. Mols. H«0.
-23 36.08
5.42 Cu(N(\),.9Hi0 20
55.58 12 Cu(N(\)t.6H^
— 20 40.92
6.65 " 26.4
63.39 16.7
-21 39.52
6 . 27 Cu(N(\)t.6H|0 25
60.01 14.4 Cu(N(^s.3^0
0 45
7 . 87 " 40
61.51 15.2
+10 48.79
9.15 " 60
64.17 17.2
18 53.86
11.20 . « 80
67.51 20
"45
77.59 33-3
Density of solution saturated at 18® ■= 1.681.
100 gms. HsO dissolve 127.4 gms. Cu(NOj)iat 20*^, in sat. sol. =1.688. (Fedotieff, 19x1-12.)
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 BroderMm, 19x54
COPPER OXALATE 272
COPPEB OXALATE (ic) CuC^^iU^.
One liter HsO dissolves 0.02364 gm. CuCiOi at 25", determined by the con-
ductivity method. (Schftier, 1905.)
COPPER OXIDE (ic) CuO.
Solubility in Aqueous Solutions at 25^.
(Jaeger, 190X.)
In Aq. Hydrofluoric Acid. In Aq. HF -h KF. In Aq. HNQ, and CHtCOOH.
Nomiality Gm. Atoms Normality Gm. Atoms Cy>t»M* Gm. Atoms
olHF. Cu per Liter. o£ HF. Cu per Liter. aoivent. Cu per Liter.
0.12 0.0307 0.12 0.0356 inCHjCOOH 0.1677
0.28 0.1164 0.28 0.06437 i^HNQg 0.4802
0.57 0.2494 0.57 0.1442
1.08 0.388 I. II 0.2451 Cu determined electrolytically.
2.28 0.463 2.17 0.25x7 ^" "'^^^^^^^^^^ '"«^""'y"^-*"y-
COPPER OXIDE (ous) CuiO.
Solubility in Aqueous Ammonium Solutions at 25".
(Donnan and Thomas, 19x1.)
The cuprous oxide was prepared by adding KOH solution to a mixture of
equal weights of CuS04.5HsO 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%. I'he 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. 11.
Cms. per 1000 Gms. Sol. Mols. per xooo Gms. SoL Cms. per 1000 Cms. SoL Mols. per 1000 Cms. SoL
Cu.
nh,.
Cu.
NH,. '
Cu.
NH,.
' Cu.
NH,.
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. 0144
27.03
0.01597
I 59
0.9890
22.61
0.01555
1.33
1.0462
32.64
0.01645
1.92
I. 0494
28.39
0.01650
1.67
1.3229
68.68
0.02081
4.04
1.3528
54.15
0.02127
3.19
X.4882
74.12
0.02340
4.36
I . 5048
72.08
0.02366
4.24
I. 6313
98.52
0.02565
556
1.5963
78.20
0.02510
4.60
I. 6981
122.40
0.02670
7.20
1.6555
102.05
0.02603
6
COPPER SULFATE CuS04.5H,0.
S(H.UBiLiTY IN Water.
(Etard. 1894; Patrick and Aubert, 1874; at 15*. Cohen. 1903; at 35** Trevor, 1891.)
Gms. CuSOi per 100 Gms. ^ Gms. CUSO4 per xoo 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
Sp. gr. of sat. solution of CuS04.^HsO in HsO at 16^ >- I*I93- (Greenish, igos^
100 gms. sat. solution in H|0 contam 20.32 gms. CUSO4 at 30^. (Schretnemakers, 191a)
• •
Solution.
Water.
0
".5
14.3
10
14.8
17.4
20
17.2
20.7
25
18.5
22.7
30
20
25
40
22.5
28.5
50
25
33.3
273
COPPER SULFATI
SOLUBILITT OF COPPRR SULPATB IN AqUBOUS SOLUTIONS OF AmMONIXTM
Sulfate at 0**.
(Engd, x886.)
MiDigram Equiv. per
xo oc. Solution.
Sp. Gr. of
SolutioDa.
Grams per
100 oc. Solution.
(NH.)«S0«. CuSO.
(NH4),S04.
CuSO*.
o 18.52
1. 144
0
14.79
5.45 20.15
1. 190
3.61
16.09
7 10.5
i.io8
4.63
8.38
7.4 9.1
1.099
4.90
7.26
8.45 6.425
I. 0815
5-59
5.13
"35 3-7
1. 071
7.51
2.9s
18.6 I. 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)
CuS04.(NH4)iS04.6H,0 + NiS04.(NH4)tS04.6H,0.
Mol. % in
Solution.
Mols. per loo
Mols. H|0.
Mol. % in Solid Phase.
CttSalt.
NiSalt:
Cu Salt.
Ni Salt.'
Cu Salt.
Ni Salt. ^
0
100
0
0.521
0
lOO
33-34
56.05
73-89
79.92
66.66
43-95
26.20
20.08
0.1476
0.2664
0.4165
0.4785
0.295
0.2089
0.1449
0.1202
10.29
30.59
52.23
78.80
89.71
69.41
47.77
21.20
100
0
1.0350
0
100
0
Solubility of Mixtures of Copper Ammonixtm Sulfate and Zinc
Ammonium Sulfate in Water at 13*^-14®.
(Fock, 1897.)
CuS04.(NH4)iS04.6H,0 + ZnS04.(NH4)tS04.6HiO.
Mol. % in SoluUon.
Mols. per loc
t Mols. H|0.
Mol. % in
Solid Phase.
' Co. Salt Zn Salt.'
Cu Salt.
Zn Salt. '
Cu Salt.
ZnSalt. '
4-97 95.03
0.0422
0.8069
2.39
97;6i
10.65 89.35
0.0666
0.5638
4.52
95 48
19.24 80.76
O.I218
O.5115
90.3
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
100 0
1.035
0
100
0
SOLUBIUTY OF COPPER SULFATE IN AQUEOUS SOLUTIONS OF MAGNESIUM
Sulfate
AT O".
(Diacon.
x866.)
Gms. per xoo Gms. HfO.
Solid Phase.
Gms. per xoo
• Gms. H|0.
Solid Phase.
CnSOi. MgSO*.
CuSO*.
MgSO*. '
0 26.37
MgS04.6H|0
12.03
15.67
CuS04.5H^
2.64 25.91
M
13.61
8.64
M
4.75 25.30
M
14.99
0
•1
9.01 23 . 30 MgSO«.6H^+CuS04.5H/)
COPPIB SX7LFATE
274
Solubility of Copper Sulfate in Aqueous Solutions of Copper
Chloride at 30®.
(SdiretDemaken, 1910.)
Gim. per 100 Gms.
£t.Sol.
Sntiil Phase.
CuS04.5HiO
a
u
u
Gms. per xoo Gms.
Sat. Sol.
Solid Phase.
CuOt. C11SO4.
0 20.32
6.58 13.62
15.68 8.93
25.67 4.77
CuCl..
39.48
42.62
43.25
43 95
CttS04:
3.21
2.90
1. 14
0
CUSO4.SH1O
"+CuCl,.2li
CuCl«.2HaO
Data for Equilibrium in Complex Systems Containing Copper Sulfate.
System. Authority.
CUSO4 + CuCli -f- (NH4)iS04 -f- NH4CI + HiO (Schxeinemaken. 1910.)
+ *' + KsS04 + KCl + HsO (Schreinemakena]iddeBaat,x9X4aO
+ " + Na,S04 + NaCl -f- HjO (Schremcinakera, 1911.)
+ LisS04 + (NH4)sS04 + HtO (Schreinemaken, 1909.)
II
II
S(x.uBiLiTY OF Copper Sulfate in Aqueous Solutions of Lithium
Sulfate
; AT 30".
(Schreinemakers, 1908, 1909.)
Gms. per 100 Gms.
Sat. Sol.
Solid Phase.
CUSO4.5H2O
a
Gms. per 100 Gms.
c
Solid Phase.
Li,S04. CUSO4.
0 20.32
3. 54 17.59
6.08 •16.10
LijSO*. CUSO4.
17.92 11.04
20.55 10.05
22.23 6.41
uS04.5HaO
" +Li2S04.HiO
Li,S04.H80 •
"94 13.55
a
23.59 3-39
u
15.72 12.14
n
25.24 0
«
Solubility of Copper Sulfate in Aqueous Solutions
of Lithium and
Other Chlorides at 25^
(Herz,
1910.)
In Lithium
Chloride.
In Potassium
Chloride.
In Rubidium
Chloride.
In Sodium
Chloride.
Gms. per 100 cc.
Sat. Sol.
Gms. per loo cc.
Sat. Sol.
Gms. per xoo cc.
Sat. Sol.
Gms. per loo cc.
Sat. Sol.
LiCl. CUSO4. '
KCl. CUSO4.
' RbCl. CUSO4.
NaCl. CuS04.'
3.10 20.oi6
4.19 23.89
0 22.34
2.10 22.41
5.93 18.78
8.75 24.92
13.22 25.02
7.72 22.76
12 17.03
17.50 29.03
14.79 24.05
Solubility of .Copper Potassium Sulfate CuKs(S04)s.6HiO in Water at 25'*.
100 gms. HsO dissolve 11. 14 gms. CuKs(S04)s. (Trevor, 1891.)
Additional data for the system Copper sulfate + Potassium sulfate + HsO are
given by Meerburg, 1909.
Data for the solubility in water of mix-crystals of copper sulfate and man-
ganese sulfate at 0° and 17**, and of copper sulfate and zinc sulfate at 12% 18^,
25*1 35% 40** and 45", are given by HoUemann, 1905-06.
275
GOPPIB 8UI.FATB
COPFKR SULFATB, MANGANESE SULFATE, MiXBD CRYSTALS AT 25^.
(Storteobecker, i9c».)
OflM. per 100 Gmt. HgO. Mob, per too Mob. HsO.
foSoT MnSOft. ^
TkkUnlc CryiUb with sH^.
20.2
19.76
O
Cu.
2.282
a. 23
13 65
II .61
9-39
6.47
3 01
31 -Sa
39-41
46.77
53-39
58 -93
CO 61.83
Monodimc Qryatab with 7H^.
9-39
6.47
0.0
46.77
53-39
67.o7±
1-54
I 31
1.06
0-73
0.34
0.0
1.06
0.73
0.0
Ma.
O
0.44
Mol.% Cu
in Soltttian.
Mol.% Ca
in Crj^ds.
3 76
4.70
5-59
6.37
7-03
7-375
5 58
6-37
8±*
100
90.5
83 -5
741
57-7
31 o
29.0
26.1
21.8
21.2
20.0
15 9
13-45*
10.27
5-0
4.6
2.31
0.0
20.0
15-9
13-45
10.27
4.6*
0.0
100
99-3
• • •
97-3
95-1
81.3
• . •
70.4
...
42.6
34-4
22.9
15.2*
10. 5
4 9
• • •
2-15
100. o
28.2
23 -5
20.8
16.0
5.8*
100
* Indicatea points of labil eqnilibtiiim.
Copper Sulfate, Zinc Sulfate, Mixed Crystals in Water at i8®.
(Stoctenbecker, 1897.)
Mob. per 100
Mob.QiO.
Mol. %,Cu
Mol. %Cu
Cu. '
7.n. '
inCiy^ab.
2.28
0
100
100
1.83
2.08
46.8
94.9
1. 41
3-60
28.1
1. 19
5 01
19.2
77-9
1.86
3 36
36.2
40.4
1.22
4.45
"■5
29 -5-31 -9
1. 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
487
7.02
0.0
6.42
0.0
0
1. 19
5.01
19. 2
5.01
0.51
5-59
8.36
1.97
0.267
5-77
4.42
i-iS
0.0
5-94
0.0
0.00
' Tridfaiic Qryatab with sH^.
•- MoBodinir Oyatali with 7H«0.
Rhombic Cryatab with 7H«0.
GOPFIB SULFATE
276
Solubility of Copper Sulfate, Sodium Sulfate Mixtures in Water.
(Koppel, 1901-oa; Muaol and Maldes, 1901.)
Solid Phase.
Gmg. per ]
Solut
[00 Cms.
Mols. per xoo Mob.
f.
ion.
I^.
'CuSO*.
NatSOi:
CUSO4.
Na,S04.
0
13 40
6.23
1.88
0.98
ID
14.90
9.46
2.23
1.56
}S
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
13.48
2.37
2.39
23
16.41
"35
2.57
1.99
40. IS
20.56
8
3.25
1.47
x8
13. S3
13.84
2.10
2.41
20
11-34
15-70
1.76
2.73
2S
6.28
21.20
0.98
3.70
30
2.607
28.38
0.43
5.21
33-9
1.47s
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
1. 57
32.09
.
^
CoSQi.sEbO'fNatSaii.ioHiO
M
CuS0|.NaiSO«3H^
CiiSO|J7aflSO«.9H^+CiiSO«.s^O
u
n
CaSO«.Na«SO|.aH|0-VNaiSQ|.zoBdO
M
CaS04J^a^4.aH^-f increasing
amts. of Na^4ZoH/)
Data for the sYSttem copper sulfate, sodfum sulfate, water, at 20*'_and 35*
are given by Massink;, 1916, 1917.
!S(H.UBILITT OF COPPBR SULFATE IN AqUBOUS SOLVTIONS OF SULFURIC
Acid at o®. (Engd, 1887.)
Milligiam
Emnv.
per 10 Gihs.
Sp. Gr. of
Solutions.
Grams
per IOC
H»S04.
CUSO4.
feS04.
CttS04.'
0
18.6
1. 144
0
14.85
4.14
17.9
1. 143
2.03
14.29
14.6
19.6
1. 158
7.16
15.65
31
12.4
1. 170
15.20
9.90
54.2
8.06
1. 195
26.57
6.43
56.25
7.75
1. 211
27.57
6.19
71.8
5
1.224
35.2
3.99
Solubility of Copper Sulfate in Aqueous Solutions of Sulfuric Acid
AT 25®. (BeU and Taber. 1908; Footc, 19x5.)
Cms. per
Sat.
100 Cms.
Sol.
Solid Phase.
4 Gms. per
100 Gms,
Sol.
Solid Phase.
H,S04.
CUSO4. '
H,SO«.
CuS04.
0
18.47
CttS04.5HyO
55.72
2.13
CuS04.3H,0+CuSO. fl^
II. 14
12.62
u
61.79
0.95
CuSO«40
25.53
5.92
M
77.93
0.17
u
36.77
3.25
M
83.29
0.15
m
42.15
2.63
M
85.46
0.19
M
47.66
2.59
M
85.76
0.43
" +CuS04
49
2.83
« +aiS04.3H^
86.04
0.40
CuSO*
50.23
2.70
CuSO«.3HiO
92.70
0.19
«
54.78
2.19
tt
277
COPPBB SULFATE
Solubility of Copper Sulfate in Methyl and Ethyl Alcohol, etc.
(de Bruyn, 1892; de Coninck, 1905.)
Solvent.
Methyl Alcohol Abs.
it
it
tt
u
%
Abs.
Ethyl Alcohol Abs.
Glycol
Glycerol
Glycerol
95% Formic Acid
Aiiby. Hydrazine
18
18
18
3
3
14.6
^S'S
15-16
18. s
Gms. per 100 Gma. Solv. SOLUBILITY IN AqUBOUS
CUSO4. CuSOi.sHtO
I. 05 15.6
0.93
0.40
13.4
I.I
7.6*
30
36.3
0.05
...f
Alcohcm- at 15*
(Schiff, 1861.)
Wt. % Gms. CuS04.5H^
AlcohoL per 100 g. Solvent.
10 IS -3
20 3.2
40 0.25
(Oasendowski, 1907.)
(Aschan, 19x3.)
(Welsh and Brodenon, 19x5.)
ord. t. 2
* Per 100 gms. solution. f decomp.
Data for the solubility of copper sulfate in methyl alcohol are given] by Carrara
and Minozzi, 1897.
COPPER SULFIDE (ic) CuS.
' One liter of water dissolves 0.00033 gm. CuS at 18*, determined by the conduc-
tivity method. (Weigel, 1906; see also Bnmer and Zawadski, 1909.)
100 cc. sat aq. sodium sulfide solution (of d = 1.225) dissolve 0.0032 gm. CuS.
(HoUand. X897.)
Solubility of Copper Sulfide in Aqueous Sugar Sco^utions.
(Stolle, 1900.)
%Sugar
m Solvent.
10
30
SO
Gms. CuS per Liter of Aq. Sugar Solution at:
X7.S*- 45*- 7S".
0.5672 0.3659 1.134s
0.8632 0.7220 1.2033
0.9076 1.0589 1.2809
COPPER SULFIDE (ous) Cu,S.
Freezing-point lowering data (solubility, see footnote, p. i) for mixtures of
CuiS -\- AgtS, CuiS + PbS and CU2S + znS are given by Friedrich, 1907-08.
Results for CutS + SbsSi are given bv Chikashigi and Yamanchi, 19 16. Data
for CusS + FeS are given by Shad and Bomemann, 1916.
COPPER SULFONATES.
100 gms. HsO dissolve 0.25 gm. copper 2-phenanthrene monosulfonate at 20'
" " " o!26 " " 10- "
COPPER TARTRATE
CuC40eH4.3HiO.
Solubility in Water.
(Canton! and Zacboder, 1905.)
II
(Sandquist, x9X3.)
f.
Gms.
CuC«ObH4.3HaO
per xoocc.
Solution.
f.
Gms.
CuC«0A-3H^
per 100 cc.
Solution.
r.
Gms.
CuC«0^H4.3H^
per xoocc
Solution.
IS
0.0197
40
0.1420
6S
0.1767
o.i64</
20
0.0420
45
0.1708
70
2S
0.0690
SO
0.1920
7S
0.1566
30
0.0890
55
0.2124
80
0.1440
3S
0.1205
60
0.1970
8S
0.1370
COPPER THIOCTANATB
278
COPPIB THIOCYANATB (ic) Cu(SCN)s.
Solubility in Aqueous Ammonia Solutions at 25^ and at 40^
SatT^l.
X.0082
I. 0166
I. 0213
1.0171
1.0151
I. 0134
1.0070
0.9987
o . 9985
Results at 25**.
Gms. per xoo Cms. Sat. Sol.
NH..
0.79
1.98
2.50
4.26
S-3S
6-39
9-93
21.47
Cu(SCN),.
2-45
4.08
S"
5-96
6.22
6-59
7.98
11.24
15.22
(Hom, 1907.)
Solid Phase.
Cu(SCN)t.2NH|
(I
II
Ctt(SCN)t.4NHt
It
II
II
(f
(I
, Results at 40^
Gms. per 100 Gms. Sat. Sol.
NH..
0.94
1.77
2-57
3S2
4. 35
SSo
7.58
13.98
18.02
Cu(SCN)».
2.81
4.18
8.76
11.78
12.07
12.99
16.58
19.76
Sdid Phase.
Cu(SCN)t.2NH|
fi
u
Cu(SCN)t4NHa
II
M
u
COUMABIN CsHeOs.
100 gms. water dissolve 0.01 gm. coumaiin at 20^-25°. (Dehn. 19x7.)
*^ pyridine " 87.7 gms.
50% aq. pyridine " 60.1 "
chloroform " 49.4 " " " 25*. (OsiJca. 1903-08.)
Freezing-point lowering data for mixtures of coumarin and sulfuric acid are
given by Kendall and Carpenter, 1914.
GRESOLS CeH4(0H)CH, 0, m and /».
Solubility of Each Separately in Water.
(At ao", Vaubel, 1895; Sidgwick, Spurrell and Davies, 19x5.)
Determinations by synthetic method; melting-point oi 0 ^ 29.9®, of m = 4",
of p = 33'^^' Triple point for 0 = 87 and 2.5 gms. per 100 gms. sat. sol. at
8**; triple point for ^ = 86 and 2 gms. per 100 gms. sat. sol. at 8.7**.
Gms. per xoo Gms. Sat. Solution.
Gms. per 100 Gms. Sat. Solution.
f.
0 Cresol.
m Cresol.
p Cresol.
f.
0 Cresol.
M Cresol.
^CresoL'
20
2-45
2.18
1.94
120
6.22
7
6.58
40
308
2.51
2.26
130
6.70
8.86
9
50
3.22
2.72
2.43
140
7.67
12.3
iS-9
60
3 40
2.98
2.69
143 . 5 crit. t.
• • •
• • •
00
70
3-74
3-35
3 03
147 crit. t.
• • •
00
80
4.22
3.80
3.52
ISO
II. I
90
4.80
4-43
4. .16
160
237
100
S-30
5-47
S-io
162.8 crit. t.
00
no
5.80
5-96
SSO
One liter aqueous i normal solution of the sodium salt of 0 cresol dissolves
7.57 gms. 0 cresol at 25°, 8.32 gms. at 40**, 9.84 gms. at 60° and 13.62 gms. at 8o*
(Sidgwick, 19x0.)
MisciBiLiTY OF Aqueous Alkaline Solutions of tn 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 tn cresol
dropwise, until solution occurred. Temp, not stated.
Composition of Homogeneous Solution.
/ * .
cc. Aq. KOH.
s
s
s
s
s
* B the nonnal secondary alcohol, the so-called capryl alcohol, CHi(CH|)«CH(OH)CB^
Aq. Insol. Cmpd.
MCnsoL
2 CC.
(i .64 gms.) Octyl Alcohol*
I.I gms.
5"
(4.1 " ) "
1.8 "
2 "
(1.74 " ) Toluene
4-4 "
3"
(2.61 " ) "
S-i "
2 "
(i .36 " ) Heptane
6.4 "
279 GRESOL
Distribution of Cresol between Water and Ether. (Vaubei, 1903.)
Composition of Solvent. ^°*** lS^J/" ^^ In Ether Uyer.
200 cc. H2O+ 100 cc. Ether o . 0570 i . 0760
200 cc. H2O+ 200 cc. Ether o . 0190 i . 1 144
Freezing-point Lowering Data (Solubility, see footnote, p. i) for Mix-
tures OF Of m AND p Cresol (each determined separately) and Other
Compounds.
Mixture. Authority.
0, m and p Cresol + Dimethylpyrone (KendaU, 1914.)
" " + Picric Acid (Kendall, 1916.)
" " -j- Pyridine (Hatcher and Skirrow, 1917.)
0 and p a ^ a (Bramley, 19x6.)
" " + Sulfuric Acid (Kendall and Carpenter. 1914.)
£», m.and P " + Urea (Kremann, 1907.)
Trinitrocresol + Naphthalene (Saposchlnikow and Gelvich, 1903, 1904.)
CROTONIC ACmS a = CH,CH:CHCOOH, /J =. HCH,C:CHCOOH.
Freezing-point Lowering Data for Mixtures of Crotonic Acids and of
Crotonic AaD and Other Compounds.
Mixture. ^ ^ Authority.
a Crotonic Acid + P Crotonic Add (MorreU and Hanson, 1904.)
" " -j- Dimethylpyrone (Kendall, 19x4.)
" "4- Sulfuric Acid (Kendall and Carpenter, 1914.)
Chlorocrotonic Acid + Dimethylpyrone (Kendall, 1914.)
" " + Sulfuric Acid (Kendall and Carpenter, 1914.)
Methyl CBYPTOPIMES, i4, 5 and C forms, C«H»OtN.
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. (Sidgrrick, 1915.)
CUMINIG ACm CtH7C«H4.COOH (/» Isopropyl Benzoic Acid).
Solubility in Water at 25**. (Paul. 1894.)
1000 cc. sat. solution contain 0.1519 gm. or 0.926 miliimol cuminic acid.
PseudoGUMIDIME (CH«)t.C«Hs.NHs (5, 5 Amino, i. 2. 4. Trimethyl Benzene).
Solubility in Water.
(Lowenherz, 1898.)
t*. 19.4". 93.7". a8.7*.
Gms. ^ Cumidine per liter H2O i . 198 . i .330 i .498
CYANAMIDE CN.NH,.
Solubility in Water, Determined by Freezing-point Method.
(Pratokmgo, 19x3.)
Gms. '
Solid Ph«e. f of CongeJirg. ^^,^^ p^.
Sat. Sol.
Ice —14.39 40.19 CN.NHi
— 2.49 56.80 "
+ 14.50 77.20
25.6 87.15
"+CN.NH. 37.90 96.77
CN'.NHt 42 . 9 100
Simila data forjZN.NHi -|- urea and^CN.NHj + dicyandiamide are also given.
DiCTANDIAMIDIME Perchlorate C2H6N4OHCIO4.
100 gms. HsO dissolve 9.97 gms. of the salt at 1 7° {d sat. sol. »> i . 039) . (Carbon, 19x0.;
t*of Congealing.
— 0.62
Gms.
CN.NH, per
xoo Gms.
Sat. Sol.
2.58
- 3.96
- 7.58
9.42
18.40
— 12.72
— 16.6 Eutec.
30.9
37.8
-15-6
38.7s
tf
(f
(I
M
M
CYANOGEN 280
CTANOOEN (CN)^
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)s. On account of polymerization, the
solubility increased with time of contact and amount of agitation of the mixture.
One volume of HsO at 30° dissolves 3.5 vols. (CN)s after 2 hours, and 9.7 vols,
after 97 hours.
One volume of abs. alcohol at 20° dissolves 26 vols. (CN)i immediately; 39
vols, after 4 hours; 89 vols, after 48 hrs. and 223 vols, after ± days.
One volume glacial acetic acid dissolves 42 vols, of (CN)s immediately and
50^ vols, after 3 days.
One volume of chloroform dissolves about 19 vols. (CN)i immediately and
29-30 vols, with time.
One volume of benzine finally dissolves 28 vols. (CN)t.
One volume of rectified turpentine dissolves 9-10 vols, of (CN)i.
One volume of ether dissolves 5 vok. (CN)i at 20®. (Gay Lusiac.)
CYCLOHEZANB (Hexamethylene, Hexahydrobenzene) CHs < (CHs.CHt)s >
CH,.
Freezing-point data (solubility, see footnote, p. i) for mixtures of cyclo-
hexane and ethylene bromide are given by Baud (l9i^b). 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, 191 o).
CTCLOHIXANOL (CHOlCHOH.
100 gms. HtO dissolve 5.67 gms. cyclohexanol at 11*^. (de Foroand, 191 3.)
100 gms. cyclohexanol dissolve 11.27 gms. HtO at II^ "
Reciprocal Solubility of Cyclohexanol and Water, Determxned by
THE Freezing-point Method.
(de Forcnnd, 1912.)
Gm. (CH0».CHOH Gm. (CH^.CHOH
i* of Solidification. per xoo Gnu. t* of Solidification. per 100 Gms.
Mixture. Mixture.
+22.45 '^^ — S7.4Eutec. 95030
17.48 99-767 -43-2 93 150
— 1.40 98.817 —33 91.962
—34.10 96.868 —18.50 90.980
—46.80 9S-9IO ~"I4SS 90.36
— 55-70 95-170 -12.05 S8.73
Freezing-point data for mixtures of cyclohexanol and phenol are given by
Mascarelli and Pestalozza, 1908, 1909.
CYCLOHIXANONE (CHOiiCO.
Freezing-point data for mixtures of cyclohexanone and phenol are given by
Schmidlin and Lang, 1910.
CmSIME (Ulexine) CnHieNjO (m. pt. ISI^^-ISI-S**).
Solubility in Several Solvents at i$\
CV'an de Moer, 1891.)
Snlvrat Gms. CnHwNjO per
bolvcnt. j^ Q^ ^^ SoL
Benzine i . 26
Petroleum Ether insol.
Amyl Alcohol o . 303
Carbon Disulfide insol.
Ethyl Acetate very soluble
Solvent
Gms. CuHx.N/)
per 100 Gms. Sat. SoL
Water
soluble in ail proportions
Alcohol
u u tt
Chloroform
C( If II
Ether {d 0.725)
0.302
Ether, abs.
insol.
28l
DEXTBIN
DSZTBIN Ci,H»Oio.
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 S™s- dextrin at 20-25°.
100 gms. aq. 50% pyridine dissolve 102 gms. dextrin at 20-25°.
(Dehn, 19x7.)
DIACKTYL TARTARIC ETHER (m. pt. 104°) DIACETTL RACEMIG
(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 CeH8.CH2.CH,.C«Hs.
Freezing-point lowering data for mixtures of dibenzyl and stilbene are given by
Garelli and Calzolari, 1899.
DIDYMIUM Ammonium NITRATE Di(NOs)i.2NH4NQi.
100 gms. HsO dis
solve 292 gms. of the salt a
ti5".
(Holinbeis. 1907-)
DIDYMIUM SULFATE Di,(S04)i.
Solubility in Water.
(Marignac, 1853.)
Gmfl. Di,(SO«)«
Cfins. Di,(S04)i
t*. per TOO
SoUd Phase. t*.
per 100
SoUdPiiaw.
Ginft.H^.
Gias. H«0.
12 43.1
DiaCSOOa ?
34.0
Dii(S04),.6H»0
18 25.8
19
II. 7
D^(SO0t.8H^
25 20.6
40
^.^
ii
38 13
!! SO
6.S
a
SO II
100
1.8
it
DIDYMIUM POTASSIUM SUIiFATE KsS04.Dis(S04}i.2HsO. (Marignac.)
100 gms. H2O dissolve 1.6 grams of the double salt at i8^
DIDYMIUM SULFONATES.
Solubility in Water. (Holmbeig, 1907.)
Salt.
F<ffmala.
f.
Didymium Benzene Sulfonate Di(C«HftSOs)s.9HsO
i» Nitro Benzene Sulfonate Di(C6H4(NOi)SO,),.6HiO
tt
«
tt
tn Chloro
tn Bromo
Chloro Nitro "
a Naphthalene Sulfonate
i.SNitro "
1.6
1.7 " "
IS
IS
Di(C«H4ClSO,),.9H,0 15
Di(CtaBrSO,),.9HtO 15
Di(C«H4Cl(NO,)SO,*),.i6H,0 15
Di(C,oH7SO,),.6H20 15
Di(CioH6(NO,)SO,),.6H,0 15
Di(C,oHe(NO*)SQ,),.9H,0 15
Di(CioH4,(NOi)SO»),.9H^ iS
Gms.
Anhydrous
Salt per 100
Gm8.H|0.
S3I
47.8
12.7
14-3
25. 3
6.1
0.52
0.18
1.3
• (S0i:N0i:a - 1.3-6.)
DIETHYLAMINE see ETHYLAMENE, page 294.
DIONINE (Ethyl Morphine) Ci»H»NOs.
100 cc. HfO dissolve 0.2613 gm. Ci0HaNOs at 20^
100 cc. oil of sesame dissolve 0.5144 gm. CuHnNOi at 20^
(Zalai, 19x0.)
DIFUINYL
282
DIPHSMTL C«Hi.C«Hi.
100 grams absolute methyl alcohol dissolve 6.57 grains 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 + phenanthrene and for diphenyl + triphenylmethane are
given by Vignon (1891).
DIPHINTLAMINS (C«H.)tNH.
RsaPROCAL SQLUBILITY of DlPHBNYLAlONB AND WaTBR, BT SYNTHETIC
f Method.
(Campetti and del GtOMo, 19x3.) '
Cms. (C«K),NH
t*. per 100 Gmi.
Mixture.
305crit. t. 47. s
304 62.52
299 73.07
289 82.08
249 86.73
Similar data for the systems diphenylamine + ether ^and diphenylamine +
iaopentane are given by Uimpetti, 1917.
SoLUBH^mr OF Difhenylaionb in Several Solvents.
r.
Gnu. (C|H|)i NH
Mixture.
231
1.48
264
3-49
27s
5.62
297
16.50
303
45.16
f.
Cms. (C«^tNH
per xoo Gms.
Mixture.
239
88.28
229
90.23
210
92.93
152
97.19
SohfenL
Water
Methyl Alcohol
t( it
Ethyl Alcohol
u
il
Propyl Alcohol
Pyridine
Aq. 50% Pyridine
M Gms. t&HOsNH
per 100 GiDB. Solvent.
20-25 0.03
145 4S-2
I9-S S7.S
14. s 39.4
19.5 56
14. S 29.4
20-25 302
20-25 two layers formed
Authority.
(Dehn, 19x7.)
(Timofeiew, 1894.)
(de Bruyn, 1892.)
(Timofeiew, 1894.)
(de Bntyn, 1892.)
(Tiniofeiew, 1894.)
(Defan, 19x7.)
u
SOLUBH^ITY OF DiFHBNYLAMINE AND ALSO OF TrIFHENYLAMINE IN CARBON
Disulfide. (Arctowtki, i895>)
NH(C:,H|), in CS,
N(CJIi), in CS,.
r.
-88i
-X17
Gms. per 100
Gms. Solution.
0.87
0.37
f.
-83
-91
— 102
-xi3i
Gms. per 100
Gms. Solution.
1. 91
1.56
1.24
0.98
SoLUBiLmr OF Diphenylamine in Hexane and in Carbon Disulfide.
(Etard, 1894.)
r.
Gms. NH(CJI.)t
per xoo Gms. Sol. in:
Hexane. CS,. ~
-60
1.3
-so
2.2
-40
... 3.8
-30
0.5 7.2
— 20
0.8 12.5
— 10
1.4 21.6
f.
o
+10
20
30
40
50
Gms. NH(C|H0^
per 100 Gms. Sol. m:
Hexane.
2.6
3.8
6.7
13.8
47
94
CS,.
33-7
46.8
60.9
76
II
II
II
283 DIPHBNYLAMINl
Freezing-point Data for Mixtures op Diphenylaminb and Other
Compounds.
Diphenylamine + Acetyldiphenylamine (Boeaeken, 1912.)
" + Ethylene Bromide (Dahms, 1895.)
" + Naphthalene (Roloff, 1895; Vignon. 189x0
+ a Naphthylamine (Vignon, 1891.)
+ Nitronaphthalene (Battdli and Martinetti, z88s0
+ a and fi Naphthol Vignon, 1891.)
" + Paraffin (Pakno and Battdli, z88i30
" 4- Phenanthrene (Narbuu, 1905.)
" + Phenol (PhiKp. 1905.)
" + Resorcinol (Vignon, 1891.)
" + p Nitrotoluene (Giua, 191s.)
" + 2.4 Dinitrotoluene "
" + a Trinitrotoluene "
" + ^ Toluidine (Vignon, 1891.)
" + Urethau (Puahin and Grebenadiikov, 19x3^
Diphenylmethylamine + Phenol (Bramlor, 19x6.)
" '\- 0 Chlorophenol
Hexanitrodiphenylamine + a Trinitrotoluene
(Giua, 19x5.)
DIPHENYLAMINE BLUE.
Scx^UBiLiTY IN Several Solvents at 23^
(Szathmaxy de Szachinar, x9xo.)
Sdvent. Gms. Diphenylamme Blue g^j ^ Gms. Diphenyluibe Blue
per 100 Gms. Sat. Sol. sfw»t«ii.. p^ ^^^ Qa^. Sat. SoL
Methyl Alcohol 0.385 Acetone o-i77
Ethyl " 0.230 Aniline 0.395
Amyl " 0.049
DIPHENYL SULFIDE (CeHi)sS, etc
Freezing-point lowering data for mixtures of (CeHi)iS + ((r6Hi)sSe, (CeHi)sS +
(CJl*),Te, (CA),S + (C«H*),0, (C«H*),Se+ (C.H*),Te, are given by Pascal (1912).
DYES.
-Data for the distribution of 12 dyes between water and iaobutyl alcohol at 25%
are given by Reinders and Lely, Jr. (19 12).
DYSPROSIUM OXALATE Dys(C,04)i.ioHsO.
100 cc. aq. 20% methylamine oxalate dissolve 0.276 gm. DyiCCsOOi.
ethylamine " " 1.787 "
triethylamine " " 1.432 "
(Grant and
James,
X9X7.)
EDESTIN and Edestin Salts.
Solubility in Aq. Salt Sch^utions at 25®.
(Osborne and Harris, 1905.)
The determinations were made by shaking an excess of the air-drv 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 ^culated 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. NaCTl.
Gms. NaCl per 20 cc. Solvent — * o . 468 o . 585 o . 702 0.818 o . 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. edestm at 20-25*^. (Dehn, X9X7.)
100 gms. aq. 50% pyridine dissdve 9.05 gm. edestin at 20-25^ "
MLkTEBJH 384
ILATIBIN CiDH«Ok.
100 cc. 90% alcohol dissolve 0.09 gm. elaterin at 15-20. (Sqoize and Cainu. 1905.)
100 cc. chloroform dissolve 4 gms. elaterin at 15-20.
EMBTZNI and Salts.
Sqlubility in Water.
(Cmt and Pyman, 1914.)
Sdt. Fonn«k. f. ^,5^^.|£
Emetine Hydrochloride CttH4o04N3. 2HCI.7H1O 18 13 . i
" Hydrobromide Ci»H4(04Ns.2HBr.4l]^ 17-18 1.9
" Nitrate Cs9H4o04N,.2HNQs.3H,0 17-18 3.7
" Sulfate CnH40O4N1.HtSO4.7HsO 17-18 more than 100
IRBIUM OXALATE Er,(CsO«),.i4H,0.
Solubility in Aq. Sulfuric Acm at 25*.
(Wiith. X9X2.)
Nonnalityof
Aq.H«SQft.
Gms. per xoo
ErA.
t Gms. Sat. Sol.
Er,(CO«),:
Solid Phase.
2.16
0.329
0.5144
Er2(Cj04)8.i4H«D
3"
0.493
0.7708
«
4.32
0 . 7036
1. 10
u
6.17s
1. 10
1.72
«
II
M
ERBIUM Dimethyl PHOSPHATE ErtECCHOsPOJe.
100 gms. HsO dissolve 1.78 gm. Ers[(CHt)sP04]4 at 25^ (Moisan aadjamea. 19x4.)
ERBIUM SULFATE Er,(S04)i.8HsO.
Solubility in Water and Aq.''HiS04 at 25*.
(Wiith. i9xa.)
,. Gms. per xoo Gms. ._ ,.^ [Gms. per xoo Gms.
Nomabty St. .Sol. Solid Phase. ^T^*^ Sat.Sol. f SoHd Phaae.
'^^^*' ErA. Er,(SO0,.- ^^•^** ErA- Er,(SOJ,.
Water alone 7. 339 11.94 £ri(S04)i.8H^ 2. 16 3.98 6.473 Ers(S04)i.8H^
O.I 7.389 12.02 « 6.17s 0.9352 I. 521
0.505 6.249 10.164 " 12.6 0.0852 0.1386
I.I 5.256 8.549
ERBIUM Bromonitrobenzene SULFONATE Er(CcHtBr.NOs.SQt, 1.4.2)1. i2HsO.
100 gms. sat. solution in water contain 6.056 gms. anhydrous salt at 25°.
(Kats ami Jamics, 1913.)
ERUCIG ACm C8Hi7CH:CH(CH,)iiCOOH.
SCO^UBILFTY IN AlCOHOLS.
(Timofeiew, 1894.)
Gms. Exude Gms. Enidc
Alcohol. t*. Acid per 100 Alcohol. t*. Add per xoo
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
Ethyl Alcohol - 2 8.24 " " 21.4 63
ERTTHRITOL (CHsOH.CHOH),.
100 gms. HjO dissolve 61.5 gms. erythritol at 20-25^ (Dehn, 19x7)
100 gms. aq. 50% pyridine dissolve 8.47 gms. erythritol at 20-25®.
too gms. pyridine aissolve 2.50 + gms. erythritol at 20-25. (Dehn,|x9x7; Holty, 1905.)
385 ETHAMI
BTHAMI
L^taR,
■i v^nc
SoLUBiLrrY IN Water.
(Winkler. 190X.)
f.
. /9-
^'.
tf. f. /5.
fi^-
ff-
o
0.0987
00982
0.0132 40 0.0292
0.0271
0.0037
5
0.0803
0.0796
0.0107 50 0.0246
0.0216
0.0029
lO
0.0656
0.0648
0.0087 60 0.0218
0.017s
0.0024
IS
0.0550
0.0541
0.0073 70 0.0195
0.0135
0.0018
20
0.0472
0.0462
0.0062 80 0.0183
0.0097
0.0013
as
0.0410
0.0398
0.0054 90 0.0176
0.0054
0.0007
30
00362
0.0347
0.0049 1^^ 0.0172
0.0000
0.0000
P = 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.
P' = Solubility, i.e., the volume of gas (reduced to o° and 760 mm.)
which is absorbed by one voltime of the liquid when the barometer
indicates 760 mm. pressure.
q = the weight 01 gas in grams which is taken up by 100 grams at
the pure solvent at the indicated temperature and a total pressure
(that is, the partial |)ressure of the gas plus the vapor pressure of tha
Uquid 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.
SoLUBiLmr OF Ethane in Several Alcohols and Other Solvents.
(McDanid, 1911.)
(«^. . j^ Ads* ' BiioflCQ c 1 & a* Ads. ouosqi
Solvent. r. Cocf.A. Coef.B. Solvent. V. Coef . A. Cocf.B.
Methyl Alcohol (99%) 22.1 0.4436 0.4102 AmylAlcx)hol 22 0.4532 0.4196
" " 30.2 0.4278 0.3883 " " 30.1 0.4444 04002
" " 40 0.3938 0.3436 Benzene 22.Z 0.4954 0.4600
" " 49.8 0.2695 0.2278 ** 35 0.4484 0.3976
Ethyl Alcohol (99.8%) 22*2 0.4628 0.4282 " 40. z 0.4198 0.3661
" " So.T 0.4503 0.4051 " 49.9 0.3645 0.3081
" " 40 0.4323 0.3771 Toluene 25 0.4852 0.4450
Isopropyl Alcohol 21.5 04620 0.4275 " 30 0.4778 0.4300
" " 29.9 0.4532 0.4081 " 40.1 0.4675 04080
" " 40 0.4400 0.3837 " 50.2 0.4545 0.4013
" " 60.3 0.4244 0.3478 ** 60 0.4502 0.3690
Abs. coef. A = vol. of ethane absorbed by unit volume of solvent at the temp, stated.
For definition of Bunsen Coef. B, see fi above, and also carbon dioxide, p. 227.
Additional data for the solubility of ethane in amyl alcohol are given by (Friedel
and Gorgeu, 1908).
BTHYL ACETATE CHiCOOCsHs.
Solubility of Ethyl Acetate in Water and Vice Versa.
(Merrunan, 19x3, see also Seidell/'igio.)
Results for Ethyl Acetate in Water. Results for Water in Ethyl Acetate.
f. rfj* of Sat. Sol. ^i^^S?^ f. rf/o£Sat.Sol. ,&^vWlJ^^^
O I 0034 II. 21
5 1.0022 10.38
10 1.0009 9.67
IS 0.999s 9 OS
20 0.9979 8.53
25 0.9962 8.08
30 0.9943 7.71
40 0.9901 7.10
V.
rfjj of Sat. Sd.
Gnu. ^Opc
Gnu. CH,C(S(
0
0.9280
2-34
10
0.9164
3.68
20
0.9054
307
2S
0.9002
3-30
30
0.8953
3S2
40
0.8863
4.08
SO
• ■ •
4.67
60
• • •
5-29
ETHTL ACETATE
286
Solubility in Water and in Aqueous Salt Solutions at 28*.
(Euler — Z. phyaik. Cbem. 3i» 365, '99; 49» 306, '04.)
Cone, of Salt
CH^OOCsHi
Cone, of Salt
CHsCOOCA
Solutioa.
P« Liter.
SolutioQ.
per
Uter.
^veat.
'Nor- Gnu- per'
maHty. liter.
Gram
Mols.
Grams.
' Nor- Gms. per
Cram
Moh.
Gram*.
Water
0
0
0.825
75.02 NaCl(at 18?)
i 14.62
0.76
67.0
KNO,
i
50.59
0.77
67.81
i 29.25
0.67
59- 0
ii
I
loi . 19
0.72
63.40 "
I 58.5
0.51
45.0
€t
2
202.38
0.625
55.04 Na2S04
I 71.08
0.465
40.96
KCl
}
18.4
0.747
65.79 " (at 18°)
4 35.54
0.61
54.0
«
i
36.8
0.685
6533 "
I 71.08
0.42
37.0
tt
I
73.6
0.575
50.64 MgSO*
I 16.30
0.733
64.55
a
a
147.2
0.41
36. II "
J 32.6
0.655
57.68
NaQ
I
14.62
0.745
65.61 "
I 65.21
0.505
44.47
€t
i
29.25
0.677
59.62 ZnS04
i 20.18
0.733
64.55
U
I
58.5
0.545
47.99 "
i 40.36
0.653
57.50
«
2
117.0
0.315
27.74 "
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, 191 3. 1
Solubility of Ethyl Acetate in Aqueous Solutions of Ethyl Alcohol at 25^
(Seidell, 19x0.)
wt. % c«h»oh
in Solvent.
d»of Sat.
Sd.
ce. CH,COOCaHt Gms. CH,C00CiH»
per 100 cc. per xoo Cms.
Solvent. Solvent.
0
0.999
10
8.6
s
0.993
10.5
95
10
0.986
12
10.9
IS
0.974
15
13-3
20
0.960
27
19.6
25
0.945
44
37 0
30
0.931
70
66.7
35
0.918
"5
132.5
40
• • •
00
00
Solubility op Ethyl Acetate in Aqueous Ethyl Alcohol, Methyl
Alcohol, and Acetone Mixtures at 20°.
(Banaolt — Phys. Rev. 3, laa, 131, '05-^96.)
In Ethyl Alcohol. In Methyl Alcohol. In Acetone.
Per X cc. CaHgOH.
Per X
cc. CHjOH.
Per X cc. (CHi)«CO.
ccHflO.*
CHgCOdCsHs.t
CC.H1O.
CHgCObCA.
OC. HiO.
CHsCOOCA.
XO
0.25
10
1.08
10
1. 01
8
0.27
3
0.68
5
0.60
4
035
1-5
1.69
2
0.43
2
1.02
1.29
2.50
1-5
0.47
X.06
2.50
I.O
4.9
1.0
0.63
0.65
S-O
0.98
7.0
0.8
0.74
0.54
7.0
1.0
8.0
0.51
1. 00
0.44
10. 0
1.03
10. 0
0.25
0.29
2.00
5.00
* Satuxatedlwitli ethyl 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 bramiey, 19 15.
287
BTH7L ALCOHOL
Reciprocal Solubility of Ethyl Alcohol and Water at Low Tem-
peratures, Determined by the Freezing-point Method.
(Pictet and Altschul, 1895; Pkkeringp 1893.)
Gms.
Gms. ■
•
f.of
Sp. Gr. CaHiOHper
Solid
f.of
Sp. Gr.
CAOHper Sdid
Freeang.
Sat. Sol.
100 Gms.
Sat. Sol.
Phase.
Freezing.
Sat. Sol.
100 Gms.
Sat. Sol.
Phase.
— I
0.9962
2.S
Ice
- 23:6
0.9512
33-8
Ice
— 2
0.9916
4.8
II
- 28.7
0.9417
39
tt
- 3
0.9870
6.8
II
- 33-9
0.9270
46.3
M
- S
0.9824
"•3
II
- 41
0.9047
56.1
M
- 6.1
0.9793
138
II
- SO
• • •
68
M
- 8.7
0.9747
17s
II
- 60
75
M
- 9-4
0.9732
18.8
II
- 70
• 1
80
«l
— 10.6
0.9712
20.3
II
- 80
• (
83. 5
M
— 12.2
0.9689
22.1
II
— 100
• 1
895
II
-14
0 . 9662
24.2
II
— ii8Eutec. .
93-5
" +CAOH
-16
0.9627
26.7
II
-"S
• 1
96 QHiOH
-18.9
0.9578
29.9
II
-iio.s
•
100
II
The result for the eutectic and for the f.-pt. of CsHiOH are by Puschin and
Glagoleva, I9i4t 1915; the other data for concentrations of CsH«OH above 70%
were obtained by exterpolation. Additional data for the freezing-point lowering
are given by Rozsa (191 1).
Freezing-point lowering data for mixtures of ethyl alcohol and hydrochloric
acid are given by Maass and Mcintosh, 1913.
The distribution coefficient of ethyl alcohol between amylalcohol and water
was found by Fontein (1910) to be 1.13 at 15.5" and 1.2 1 at 28®.
Misobility of Ethyl Alcohcx. with Mixtures of:
Benzene and Water at 15®.
(Bomter, 1910.) (See also, p. 135.)
Composition of Homogeneous Mixtures.
Benzaldehyde and Water at o^
(Bonner, 1910.)
•
Composition of HomoKeneous Mixtures.
Gms.
Gms.
Gms.
Sp. Gr. of
CHiCHO.
H,0.
r,H,0H.
Mixture.
0.957
0.043
0.159
1.02
0.898
0.102
0.283
1. 01
0.800
0.200
0.420
0.99
0.700
0.300
0.550
0.98
0.598
0.402
0.601
0.97
♦0.570
0.430
0.610
• V •
0.496
0.504
0.643
0.96
0.394
0.606
0.681
0.9s
0.298
0.702
0.701
0.9s
0.200
0.800
0.670
0.9s
O.IOO
0.900
0.610
0.96
0.031
0.969
0.461
0.97
Gms.
C.H..
0.987
0.937
^0.900
0.800
0.700
0.600
0.500
0.400
0.300
0.201
O.IOO
0.020
Gms.
HtO.
0.013
0.063
O.IOO
0.200
0.300
0.400
0.500
0.600
0.700
0.799
0.900
0.980
Gms.
CaH»0H.
0.170
0.356
0.500
0.860
0.910
1.07
1. 18
1.22
I. 21
113
0.97
0.59
Sp. Gr. of
Mixture.
0.86
0.87
0.86
0.86
0.88
0.87
0.87
0.88
0.89
0.89
0.92
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, designate 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 2^^
was found bv Morgan and Benson (1907) to be 1.16. Additional data for this
system are also given by Bubanovic, 1913 and by Taylor (1897).
BTH7L ALCOHOL
288
'MisasiLiTY OF Ethyl Alcohol (see Note, p. 287) with Mixtures op:
Bromobenzene and Water
ato*.
Nitrobenzene and Water at 15*.
(Bonner,
19x0.)
(Bonner, 19x0.)
Coiii|)osition of Homogeneous Mixtures.
r
Gms.
Gms.
Gms.
Sp. Gr.
Gms.
Gms.
Gms.
Sp. Gr.
C|H«Br.
HjO.
CH»0H.
Sat. Sol.
CH,N0i.
H«0.
CH,0H.
Sat. Sol.
0.99
O.OIO
o.iis
1-34
0.96s
0.03s
0.248
1.08
'0.96
0.040
0.32
• « •
*o.9i
0.09
0.49
• • •
0.90
O.IO
0.65
1.07
0.90
O.IO
0.53
1.02
0.80
0.20
I
0.96
0.80
0.20
0.86
0.97
0.70
0.30
1. 19
0.96
0.70
0.30
1.09
0.94
0.60
0.40
1.30
0.98
0-594
0.406
1.238
0.93
O.SO
0.50
I 39
0-9S
0.50 ,
O.SO
I-3I
0.92
0.40
0.60
I 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
0.20
0.80
1.36
0.93
0.194
0.806
1. 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
0.92
0.02
0.98
0.601
0.9s
MisciBiLiTY OF Ethyl Alcohol (see Note, p. 287) at o* with Mixtures of:
Benzyl Acetate and Water. (Bonner, 19x0.) Benzyl Alcohol and Water. (Bonner, 19x0.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms. CHs."
Gms.
Gms.
sp. Gr.
Gms.
Gms.
' Gms.
Sp. Gr.
CO^.CH|.<^
I. H,0.
CHjOH.
Sat.Sol.
QH,CH/)H.
H/>.
r,H,0H.
Sat. Sol.
0.977
0.023
0.120
I. OS
0.90
O.IO
0.13
1.03
0.901
0.099
0.317
1.03
0.80
0.20
0.26
I
0.80
0.200
0.46
0.99
0.70
0.30
0.3s
0.98
0.70
0.300
o.s8
0.97
0.60
0.40
0.39
0.98
♦0.68
0.32
0.60
• • •
O.SO
0.50
0.40
0.97
0.60
0.40
0.69
0.9s
0.40
0.60
0.41
0.97
o-so
O.SO
0.78
0.94
*o.38
0.62
0.42
• * •
0.40
0.60
0.8s
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
0.3s
0.98
0.041
0.959
0.66s
0.9s
0.04
0.96
0.139
0.99
MisaBiLiTY of Ethyl Alcohol (see Note, p. 287) at 0° with Mixtures of:
Benzylethyl Ether and Water.
(Bonner, 1910.)
ConvxiBition of Homogeneous Mixtures.
* ^
Sp. Gr.
Sat. Sol.
0.94
0.92
0.92
0.91
• • •
0.91
0.91
0.92
0.92
0.92
0.93
0.94
Carbon Tetrachloride and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Gms.
Gms.
Gms.
CfH^CHs.O.CA' H,0.
CHsOH.
0.971
0.029
0.189
0.90
O.IO
0.37
0.80
0.20
0.54
0.70
0.30
0.67
♦0.67
0.33
0.71
0.60
0.40
0.78
0.50
O.SO
0.87
0.40
0.60
0.93
0.30
0.70
0.96
0.198
0.802
0.952
O.IO
0.90
0.86
0.08
0.92
0.793
Gms.
CCI4.
0.961
0.928
"0.92
0.90
0.80
0.70
0.60
0.499
0.40
0.2s
O.IO
0.032
Gms.
H,0.
0.039
0.072
0.08
O.IO
0.20
0.30
0.40
0.501
0.60
0.75
0.90
0.968
Gms.
CH»0H.
0.224
0.347
0.39
0.45-
0.67
0.82
0.94
1.04
I
i.ios
I
0.745
Sp. Gr.
Sat. SoL
1.36
1^-23
• • •
1.20
I-I5
1.07
I 03
I
0.97
0.95
0.92
0.93
289
ETH7L ALCOHOL
Distribution of Ethyl Alcohol at 25^ (Bugarszky, 1910) Between:
Bromobenzene and
Water.
Cms. CtHfcOH per Liter.
QHftBr Layer. HfO Layer.
0.72 18.5
1.36 36 -9
2.68 68.2
Carbon Tetrachloride and
Water.
Gms. CH>OH per Liter.
ecu Layer. H«0 Layer.'
0.45 18.7
0-93 36.5
2.55 68.1
Carbon Disulfide and
Water.
Gma. CiH^H per liter.
CS| Layer. H^ Layer.
0.27 19. I
I 87 37.
10.23 69.3
MisaBiLiTY 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.
Gms.
CHCna.
0.907
0.90
0.80
0.70
OS93
0.501
^0.420
0.404
0.300
0.197
O.IOO
0.088
Gms.
H«0.
0.093
O.IO
0.20
0.30
0.407
0.499
0.58
0.596
0.70
0.803
0.90
0.912
Gms.
CAOH.
0.434
0.45
0.60
0.68
0.726
0.729
0.73
0.733
0.70
0.672
0.61
0.608
Sp. Gr.
Sat. Sol.
1. 19
1. 18
1. 12
1.07
1.04
1.03
« • ■
1. 01
0.99
0.98
0.98
0.98
Gms. Gms.
CaHi.C0.CsH«. H^.
0.938 0.062
0.900
0.895
0.800
0.781
0.702
0.600
0.547
0.499
0.458
0.407
O.IO
0.105
0.20
0.219
0.298
0.400
0.453
0.501
0.542
0.593
Gms.
CAOH.
0.136
0.19
0.201
0.31
0.317
0.356
0.392
0.410
O.4II
0.415
0.404
Sp. (jr.
Sat. Sol.
0.85
0.85
0.86
0.87
0.87
0.88
0.89
0.90
0.91
0.92
0.91
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, 19x4; Bonner, 19x0; see ilso Krenuum, xgxoa.)
Composition of the Lower Layer.
Composition of Upper Layer.
Gms.
Gms.
Gms.
Sp. Gr.
Gms.
Gms.
Gms.
Sp. Gr.
(C,H,)i0.
HA
r,H,0H.
Sat. Sol.
(C,H.),0.
h^.
CH.0H.
Sat.SoL
O.IO
0.90
0.163
0.970
• • •
...
• • •
• • •
• . .
• • •
• • •
• « •
0.9S7
0.043
O.151
0-7S7
0.16
0.84
0.297
0.9SI
0.902
0.098
0.230
0.778
0.178
0.822
0.318
0.94s
0.87
0.13
0.26
0.788
0.192
0.808
0.332
0.941
0.85
o.iS
0.275
0.794
0.204
0.796
0.34
0-937
0.825
0.17s
0.292
0.800
0.227
0.773
0.352
0.932
0.79
0.210
0.313
o.8n8
0.250
0.7s
0.36
0.926
0.7S9
0.243
0.33
0.815
0.293
0.707
0.37
0.916
0.70
0.30
0.3s
0.827
0.33s
0.665
0.37s
0.906
0.645
0.3SS
0.366
0.839
0.422
0.578
0.38s
0.886
0.562
0.438
0.385
0.857
^0.49
0.51
0.385
0.874
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 conjugate
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 CaClt.6HiO are given by Morgan and Benson (1907).
STHTL ALCOHOL
290
MisaeiLiTT OF Ethyl Alcohol with Mixtures op Ethyl Ethbr and
Water at 25**. (Hariba, 1911-12.)
Compomtion of Lower Layer.
Gms.
Gms.
5-77
6.3
9423
8S-7
7.2
8
79.2
76
9-7
13 -3
70.4
62.8
22.1
50.6
28.4
•31 -6
43-4
40
Gnu. CiH^H.
O
8
13 -6
16
19.9
239
273
28.2
28.4 (Plait point)
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 eacn 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, 1910a.
Miscibility of Ethyl Alcohol (see Note p. 287) at o® with Mixtures of:
CompodtioD of Upper Layer.
Gms.
Gms.
Gms.
iCtBUfi.
H4O.
CAO.H.
98.72
1.28
0
945
2.3
3-3
88.5
3-7
7.8
84.4
4-9
10.7
75-1
8.4
16. s
60.8
iSS
23-7
43-8
28.1
28.1
35 -8
35-6
28.6
31.6
40
28.4
Ethyl Acetate and Water. (Bonner. 1910.)
Composition of Homogeneous Mixtures.
Ethyl Bromide and Water. (Bonner, xgxa)
Composition of Homogeneous Mixtures.
., A ^
Gms.
CHiaXX^iHf.
0.92
0.90
0.799
0.699
0.60
0.50
♦0.48
0.40
0.30
0.197
0.102
Gms.
H,0.
0.080
O.IO
0.201
0.301
0.40
0.50
0.52
0.60
0.70
0.803
0.898
Gms.
c,h,oh.
O.IOO
0.13
0.228
0.265
0.29
0.30
0.30
0.31
0.31
0.282
0.143
Sp. Gr.
Sat. SoL
0.91
0.91
0.93
0.92
0.9s
0.9s
• ■ ■
0.96
0.96
0.97
0.99
Gms.
QHftBr.
0.967
0.90
♦0.83
0.80
0.70
0.60
0.50
0.40
0.30
O.IO
0.017
Gms.
0.033
O.IO
0.17
0.20
0.30
0.40
0.50
0.60
0.70
0.90
0.983
Gms.
QHtOH.
0.240
0.37
0.4s
0.51
0.64
0.7S4
0.83
0.89
0.89
0.73
0.182
Sp. Gr.
Sat. SoL
1.23
IIS
• ■ •
1.09
1.06
1.03
I
0.99
0.97
0.97
0.99
Miscibility of Ethyl Alcohol (see Note p. 287) at o®, with Mixtures of:
Ethyl B u tyrate and Water. (Bonner, 19x0.) Ethyl Propionate and Water. (Bonner. xgioO
Composition of Homogeneous Mixtures.
Gms.
CiHfCCX^CfHii.
0.97
0.90
0.80
0.70
O.S99
0.494
♦0.46
0.40
0.297
0.193
O.IO
Gms.
0.030
O.IO
0.20
0.30
0.401
0.506
0.54
0.60
0.703
0.807
0.90
Gms. '
CH«0H.
0.166
0.32
0.483
0.567
0.628
0.659
0.67
0.69
0.693
0.684
0.63
Sp.Gr.
Sat. SoL
0.96
• • •
0.88
0.89
0.90
0.91
■ • •
0.92
0.93
0.94
0.94
C>>mposition of Homogeneous Mixtures.
/ ■ * ■*
Gms. Gms. Gms. Sp. Gr.
C,H,C(X)CN,. HjO. QHjOH. Sat. Sol.
0.977 0.023 0.138 0.90
0.90 O.IO 0.27 0.90
0.80 0.20 0.38 0.90
0.695 0.305 0.453 0.92
0.60 0.40 0.49 0.91
0.50 0.50 0.52 0.92
♦0.46 0.54 0.53
0.398 0.602 0.532 0.93
0.30 0.70 0.55 0.94
0.201 0.799 0.517 0.95
O.IO 0.90 0.46 0.96
n^
RHYL AljQQiMttL
MismmjTT OP Ersn. Alcobol (see Noce» p^ 1S7) at o* wtra Klixtvitss or;
Ethylene Chloride and Water.
Ethylii
iene Chlonik and
Water.
(BOHMff.
1910.)
IBOHM
lff» tj^toj
tiOBOfHoM
B^BMBOMs jfndbncs.
Gw. Godk
MVtMMlM
iitwi«.
Gw.
Gw.
Sp.Gr.
i^i^
^CLc^a
L HA
CAOH.
Stt.SoL
O^CHCV
HA
CAOH.
$fti.s»a.
0.971
0.029
O.I9I
I IS
0.98s
0.015
O.22O
I. to
0.90
O.IO
0.42
1.08
0.90
O.IO
0.43
1.03
^,88
0.12
0.46
% « %
o.Sos
0.19s
O.SvS6
I.Ot
0.792
0.208
0.670
1. 01
0.70
0.30
0.(>Q
o.qS
0.70
0.30
0.80
0.98
^).67
033
0.72
% « «
0.60
0.40
0 93
0.96
0.60
0.40
0.77
0.96
0.50
0.50
0.99
0.9s
0.50
0.50
0.82
oos
0.40
0.60
1. 01
0.94
0.437
o.S<^3
0.857
0.Q4
0.30
0.70
0.99
0.94
0.30
0.70
0.88
0.03
0.20
0.80
0.9s
0.94
0.20
0.80
0.86
0.03
0.09s
0.90s
0.842
0.96
O.IO
0.90
0.79
0.94
0.02
0.980
OSH
0.97
0.03
0.97
0.576
0.9s
MisQBiuTT OF Ethyl Alcohol C
Heptane and Water. (Bomicr, 1910.)
CompoaitioD of Homogeneoaa Mixtures.
Note, p. 287) AT o* WITH Mixtures or:
Hexane and Water. (Boomt. 1910O
Gms.
0.962
0.90
0.798
0.70
0.60
0.50
0.40
0.30
0.196
0.093
Gms.
0.038
O.IO
0.202
0.30
0.40
0.50
0.60
0.70
0.804
0.907
Gms.
CiHiOH.
0.704
1.44
2-37S
2.82
3.06
3.16
317
3 10
2.96
2.305
Sp. Gr.^
Sat. Sol.
0.79
0.80
0.82
0.81
0.82
0.83
0.84
0.85
0.87
0.88
CompositkMi of Hom«««MOua Mixtum.
Gms.
Gms.
Gms.
s^ Of.
Hcxan^.*
H|0.
C,H«OH.
SstSo).
0.97
0.03
0.59
• » *
0.90
O.IO
X'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
0.8a
0.50
0.50
2.93
0.83
0.40
0.60
300
0.83
0.20
0.80
2.7s
0.85
O.IO
0.90
2.23
0.86
0.014
0.986
1.056
• • •
Kshlbaum's Heptane and Hexsne "sus Petroleum " were used.
MisaBHjTY OP Ethyl Alcohol (see
laoamyl Alcohol and Water.
(Bonner, 19x0.) •
Note, p. 287) AT 0* WITH Mixtures or:
l8obutyl Alcohol and Water.
(Bonner, 1910.)
Composition of Homogeneous M istum.
Gms. (CILV
Gms.
Gms.
Sp. Gr.
Gms. (CH,)|
CH.CH/)H
Gms.
GmM.
Hp. (ir.
. H,0.
CH,OH.
Sat. Sol.
. H,().
C|II»()H.
Sat. Sol.
0.903
0.097
O.I16
0.84
0.70
0.30
0.13
0.87
0.90
O.IO
0.12
0.84
0.589
O.4II
0.177
0.89
0.797
0.203
0.258
0.85
0.502
0.498
0.194
0.90
0.694
0.306
0.396
0.86
0.50
0.50
0,20
0.90
0.602
0.398
0.427
0.88
0.40
0.60
0.20
0.92
0.497
0.503
0.449
0.89
0.387
0.613
0.204
0.92
0.399
0.601
0.4S3
0.90
*o.3S
0.65
0.21
• • •
0.294
0.706
0.434
0.92
0.304
0.696
0.205
0.94
*0.27
0.73
0.43
• . *
0.30
0.70
0.21
0.94
0.196
0.804
0.411
0.94
0.20
0.80
0.20
0-9S
O.IO
0.900
0.369
0.96
0.132
0.868
0.189
0.96
ETHTL ALCOHOL
292
MisaeiLiTY OF Ethyl Alcohol (see
Isoamyl Bromide and Water. (Boaner/io,
Composition of Homogeneous Mixtures.
Note, p. 287) AT O® WITH MlXTURBS OF:
.) Isobutyl Bromide and Water. (Bomwr, 'la)
Composition of Homogeneous Mixtures.
Gms.
Gms.
Gms.
Sp. Gr.
Gms. (CH|)r
CiHuBr.
H,0. QHiOH.
Sat. Sol.
CHCHsBr.
0-97S
0.025 (
0.251
1. 10
0.976
♦0.96
0.04 <
0.36
• • ■
*o-93
0.90
O.IO <
3.68
1. 01
0.90
0.80
0.20
1.09
0.96
0.80
0.70
0.30
1-37
0.94
0.70
0.60
0.40
1-57
0.93
0.60
0.498
0.502
1.676
0.91
0.501
0.40
0.60
t.7S
0.91
0.40
0.30
0.70
1-75
0.91
0.30
0.20
0,80
1. 71
0.91
0.20
O.IO
0.90
[.46
0.92
O.IO
0.022
0.978 :
[.027
0'93
0.047
Gms.
H«Q.
0.024
0.07
O.IO
0.20
0.30
0.40
0.499
0.60
0.70
0.80
0.90
0-9S3
Gms.
CAOH.
0.200
0.42
0.52
0.83
I 05
I. 21
1.30
I -35
1.36
1.32
1.20
0.937
Sp.Gr.
Sat.SoL
1. 18
1.09
1. 01
0.98
0.96
0.94
0-93
0.93
0.92
0.93
0.94
Misasn^iTY of Ethyl Alcohol (see
Isoamyl Ether and .Water. (Bonner, 'xo.)
Composition of Homogeneous Mixtures.
Note, p. 287) AT' O® WITH MlXTURBS OF!
Mesitylene and Water. (Bonner, 'zo.)
O>mposition of Homogeneous Mixtures.
Gms. r(CH«)i
Gms.
Sp. Gr.
Gms.
Gms.
Gms.
Sp. Ck.
CH.CH,CHJ,0. H,0.
CHjOH.
Sat. Sol.
CWCCH,),.
HiO.
QHaOH.
Sat.SoL
0.958
0.042
0.368
0.81
♦0.97
0.03
0.48
• • ■
0.90
O.IO
0.70
0.82
0.963
0.037
0.516
0.86
♦0.89
O.II
0.74
• • •
0.90
O.IO
1.09
0.85
0.879
O.I2I
0.793
0.82
0.80
0.20
1.66
0.84
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
0.8s
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
M1SCIBU.1TY OF Ethyl Alcohol (see
Methyl Aniline and Water. (Bonner, '10.)
' ' (imposition of Homogeneous Mixtures.
Note, p. 287) AT o® WITH Mixtures of:
Phenetoi and Water. (Bonner, 'zo.)
Composition of Homogeneous Mixtures.
Gms.
CHjNHCA
Gms.
H,0.
Gms.
CAOH.
Sp. Gr.
Sat. Sol.
Gms.
C|Hi0C|Hi|.
Gms.
Hrf).
Gms.
CHjOH.
Sp. Gr.
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
•0.90
O.IO
0.55
• • .
0.795
0.70
0.205
0.30
0.555
0.68
0.93
0.93
0.897
0.798
0.103
0.202
0.554
0.916
0.93
0.90
♦0.66
0.60
0.34
0.40
0.72
0.76
...
0.93
0.70
0.60
0.30
0.40
1. 18
1-39
0.90
0.89
0.50
0.40
0.50
0.60
0.84
0.89
0.93
0.93
0.49s
0.399
0.505
0.601
1. 518
1.560
0.89
0.89
0.30
0.20
0.70
0.80
0.91
0.87
0.93
0.94
0.30
0.198
0.70
0.802
1.54
1.449
0.90
0.91
0.098
0.041
0.902
0.959
0.734
0.581
0.95
0.96
O.IO
0.082
0.90
0.918
1. 21
1.156
0.92
0.93
293
BTHTL ALCOHOL
MisoBiLiTY OP Ethyl Alcohol (see
Pinene and Water. (Bonner, 19x0.)
Compostioii d Homogeneous Miztuies.
Note p. 287) AT o* WITH Mixtures of:
Propyl Bromide and Water. (Bonner. 19x0.)
O>mpo8ition of Homogeneous Mixtures.
Gms.
CmHn.
0.99
♦0.985
0.897
0.79s
0.70
0.60
0.493
0.393
0.293
0.194
0.094
0.03s
Gms.
H^.
O.OIO
o.ois
0.103
0.205
0.30
0.40
0.507
0.607
0.707
0.806
0.906
0.965
Gms.
CiHiOH.
0.268
0.47
I 595
2.268
2.67
2.94
3 135
3.126
3 038
2.799
1.639
Sp. Gr.
Sat. SoL
0.87
• • •
0.85
0.84
0.84
0.85
0.85
0.86
0.86
0.87
0.89
0.91
Gms.
CHs.CHg.CH(|Br*
0.97s
•0.92
0.90
0.80
0.70
0.60
0.50
0.40
0.30
0.204
0.096
0.027
Gms.
H^.
0.025
0.08
O.IO
0.20
0.30
0.40
0.50
0.60
0.70
0.796
0.904
0.973
Gms.
CAQH.
0.190
0.42
0.50
0.72
0.88
1. 01
1. 10
IIS
1. 14
1. 12
1.02
0.687
Sp. (jr.
Sat. SoL
1.26
1. 12
1.06
1.02
0.99
0.98
0.96
0.9s
0.94
0.94
0.9s
MisasiLiTY OF Ethyl Alcohol (see
Toluene and Water. (Bonner. 1910.)
Composition of Homogeneous Mixtures.
Note p. 287) AT o® WITH Mixtures of:
0 Toluidine and Water. (Bonner. 19x0.)
Composition of Homogeneous Mixtures.
Gms.
C|HtCHi*
0.948
0.90
0.80
0.70
0.60
0.50
0.40
0.30
0.20
O.IO
0.028
Gms.
H«0.
0.052
O.IO
0.20
0.30
0.40
0.50
0.60
0.70
0.80
p. 90
0.972
Cims.
CiHiOH.
0.388
0.61
0.9s
.21
.41
•53
•S9
.56
.44
•23
0.817
Sp. Gr.
Sat. Sol.
0.87
0.86
0.86
0.86
0.86
0.87
0.87
0.88
0.89
0.91
0.94
Gms.
CH,.CJI«.NI^
0.9S4
0.90
0.80
0.70
0.60
0.50
0.40
0.30
0.20
0.098
0.027
Gms.
H«Q.
0.046
O.IO
0.20
0.30
0.40
0.50
0.60
0.70
0.80
0.902
0.973
Gms.
QHfOH.
0.025
0.21
0.32
0.41
0.4SS
0.48
0.50
0.50
0.49
0.462
0.262
Sp. Gr.
Sat. Sol.
1. 01
0.93
0.97
0.96
0.96
0.96
0.96
0.96
0.96
0.98
MisciBiLiTY OF Ethyl Alcohol (see
Bromotoluene (b. pt. 182-3) and Water.
(Bonner, x9xo.)
Composition of Homogeneous Mixtures.
Note p. 287) AT o® with Mixtures of:
p Nitrotoluene and Water.
(Bonner. x9xo.)
Composition of Homogeneous Mixtures.
Gms.
BrCfiii.CHt.
0.98
0.951
0.90
0.80
0.70
0.60
0.50
0.40
0.30
0.20
O.IO
0.053
Gms.
H,0.
0.02
0.049
O.IO
0.20
0.30
0.40
0.50
0.60
0.70
0.80
0.90
0.967
Gms.
CHiOH.
0.33
0.522
0.87
.28
•54
.71
.81
.89
.89
.78
•533
•307
Sp. Gr.
Sat. Sol.
1.09
1.06
0.97
0.94
0.93
0.92
0.91
0.90
0.90
0.91
0.92
Gms.
NO,.CJI«.CH|.
0.978
*o.9S
0.90
0.80
0.70
0.60
0.506
0.398
0.294
0.20
O.IO
0.056
Gms.
H,0.
0.022
0.05
O.IO
0.20
0.30
0.40
0.494
0.602
0.706
0.80
0.90
0.944
Gms.
CHfOH.
0.253
0.50
0.84
.29
•57
•73
.782
.868
.816
.63
•30
.105
Sp. Gr.
Sat. Sof.
1.08
0.97
0.96
0.92
0.91
0.91
0.91
0.91
0.91
0.92
0.93
ETHYL ALCOHOL
294
MisaeiUTY of Ethyl Alcohol (see Note p. 287) at o® with Mixtures of:
0 Xylene and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
m Xylene and Water. (Bonner, 1910.)
Composition of Homogeneous Mixtures.
r"
Cms.
Gms.
Gms.
Sp. Gr.
r
Gms.
Gms.
Gms.
Sp. Gr.
0 C4H4(CH^«.
HtO.
C,H/)H.
Sat. Sol.
m CaH«(CH«)s.
H,0.
CHiOH.
Sat. Sol.
0.971
0.029
0-3S2
0.89
0.967
0.033
0.388
0.88
*o.96
0.04
O.S3
• • •
0.90
O.IO
0.81
0.87
0.90
O.IO
0.93
0.87
0.80
0.20
1.30
0.85
0.786
0.214
1.32
0.87
0.70
0.30
1. 61
0.86
0.70
0.30
1.53
0.87
0.60
0.40
1.77
0.86
0.60
0.40
1.72
0.87
0.50
0.50
1.90
0.87
0.50
0.50
1.87
0.87
0.40
0.60
1.98
0.87
0.40
0.60
1.96
0.88
0.30
0.70
2.01
0.88
0.30
0.70
1.94
0.88
0.20
0.80
1.87
0.89
0.20
0.80
1. 81
0.89
O.IO
0.90
1-53
0.90
0.031
0.969
1. 19
0-93
0.023
0.977
1. 168
0.92
Additional data for the system ethy
63** and 100** are given by Holt and B
1 alcohol, m xyl
ene, water at 0®,
I9'. 41%
>ell, 19 1 4.
p Xylene and
Water. (Bonner, zgzo.)
(}ompo8iti<
>n of Homogeneous Mixtures.
• V
Gms. Gms. Sp. Gr.
Composition of Homogeneous Mixtures.
A
Gms.
Gms.
Gms.
Gms.
Sp. Gr.
P CH4(CH,),.
H«0.
CH,0H.
Sat. Sol.
^C»H«(CH,),.
Hrf).
CH,0H.
Sat. Sol.
0.966
0.034
0.306
0.84
0.50
0.50
1.68
0.86
•0.92
0.08
O.S7
• • ■
0.40
0.60
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 OS
0.85
0.193
0.807
1.625
0.88
0.70
0.30
I -35
0.85
O.IOO
0.90
1-39
0.89
0.60
0.40
1.56
0.8s
0.015
0.985
0.863
_ "I 1
0.93
0.026 at 3** and 0.047 at 30®. (Meyer, 1901; 1909.)
100 gms. cottonseed oil (0.922 Sp. Gr.) dissolve 22.9 p;ms. ethyl alcohol at 25®.
100 gms. ethyl alcohol dissolve 1 1 .75 gms. cottonseed oil at 25®. (Wroth and Rcid, '16.)
Distribution of Ethyl Alcohol between Cottonseed Oil and
Water at 25®. (Wroth and Reid, 1916.)
Gms. CaHiOH per 100 cc. _ ,
Oil Layer.
H,0 Layer.
Kauo.
0.2083
6.147
29s
0.2251
6.738
29.9
0.2515
6.835
27.1
0.2783
6.876
24.7
0.3017
8.682
28.7
Data for the reciprocal solubility of ethyl alcohol and turpentine are given by
V^zes and Mouline, 1904, 1905-06.
Data for the system ethyl alcohol, water, petroleum are given by Rodt (191 6).
BTHYLAMINES C>H«.NH>, (CsHOsNH, (CsH5),N.
Freezing-point data (solubility, see footnote, p. i) for mixtures of ethylamine -|-
water, diethylamine + water, and triethylamine + water are given by Guthrie,
188^ 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:
*_;-. Vapor Pressure in Ostwald Solubility Bunsen Absorption
^^™*°*- mm. Hg. Ex. / (sec p. as?.) Coef. (see p. 227)
C2H5NH2 64.5 321 263
(CaH6)2NH 233 89 73
Data for the solubility of triethylamine in water at high pressures are given by
Kohnstamm and Timmermans, 1913.
295
ETHTLAimiiS
Solubilities op Di Ethtl
Amine and Water *
CUttey — Pha. liag. [6] lo^ 398. '05.)
Distribution op Tri Ethyl Amine
BETWEEN Water and Amyl
Alcohol at 25°.
(Hen and Fischer — Ber. 37, 4751, '04.)
Gms. NH(CsHa)s
per 190 Gms.
Gms. N(CtH8)s
per 100 cc.
Minimols N(CsH8)a
per zo cc.
f.
'Aqueous
Layer.
Amine
Layer.
Aqueous
Layer.
Alcoholic
- Layer.
Aqueous Alcoholic
Layer. Layer.
X48
146
21.7
23.6
24.8
26.3
59 0
555
53 5
51.0
0.0885
0.1683
0.1866
2.299
4-457
4.922
0.0875 2.273
01664 4.408
0.1846 4.868
MS
28.0
49.0
0.2502
6.491
0.2474 6.41S
144
31.0
45 0
143.5 (crit. t.) 37.4
TriethylAMINE N(CsH.)s.
Solubility in Water.*
(Rothmund, 1898.)
Gms. N(CaHt)i per xoo Gms.
«..
Gms. N(CtH^i per zoo Gtna,
*• r
Aq. Layer.
Amine Layer.
Aq. Layer. Amine Layer
18.6 (crit. temp.)
519
40
3.65 96.48
20 14 . 24
72
SO
2.87 96.4
25 730
95 18
ss
2.57 0-3
30 5-^
96.60
60
2.23 96.3
35 458
96 s
6s
1.97 96.3
Solubility of Triethylamine in Water and in Aq. Ethyl Alcohol
AT Different Temperatures.*
(Meerbuig, Z903.)
Water.
13-33% Alcohol.
, Gm.N(CA),
>S.98% Alcohol.
,' Gm.N(CA)i
.^8.84% Alcohol.
Gm. N(CHi)a
6o.t6% Alcohol.
Gm.N(C|H«),
Gm. NCCHi!
f.
per 100
(<ma. SoL
t*.
per xoo
Crms. SoL
t*.
per zoo
Gms. Sol.
per zoo
[?ms. Sol.
t*. per zoo
Gms. SoL
69.2
1.7
38.3
8.2
S4S
22.8
73-4
31.2
76-77 71.2
30.8
5.6
317
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
18.7
25.8
26.4
30.6
314
63.7
42.1
50.6
18.7
37-2
24.9
40.5
30-3
68.5
40.9
54.7
19s
51.8
24.2
49.8
28.5
82.2
34-2
70.6
20.5
68.6
24.1
60.7
3S
91.8
33
77.5
20.5
84
24
69.7
34.7
88
i
20.5
89.7
235
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(C)flHi)i at 19.5®.
100 gms. abs. ethyl alcohol dissolve 56 gms. NH(C«Hi)s at 19.5^.
(de Bruyn, z89a0
• Determhiadoiis znade by " Synthetic Method/' see Note, p. x6.
ETHTLAMZim 296
Distribution op Ethylaminbs Between Water and Toluene.
(Moore and Winmill, 1912.)
Results at I8^ Results at 25^ Results at 32.35^.
a™„* ^SfrfS!!;''- Partition- ^^gJS''' Petition ^Sl£?S''- Partitioa
(CsH6)NHs 0.0756 26.09 O.IIS9 19.13 0.1287 14.76
'* 0.0886 26.14 0.0999 19. II 0.2479 14.79
(CsH6)sNH 0.0484 2.14 0.0483 1.59 0.1200 1.093
" 0.0503 2.14 0.0416 1.59 0.1104 1.095
(CiHfi)8N 0.0189 0.131 0.0104 0.099 0.0132 0.069
" 0.0191 0.131 0.0131 0.099 0.0133 0.069
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, KCl, KtCOi, K2SO4 and KSCN,
are given by Timmermans (1907).
ITHTL, DiETHTL and TriETHTLAlONE HTDBOCHLOBIDES, etc. ,
Solubility of Each in Water and in Chloroform at 25®.
^ ' (Peddk and Turner, 19x3.)
Solubility in Water. Solubility in CHCU.
Amine Salt. Formula. Gms. Amine Salt Cms. Amine Salt
per xoo Gms. H|0. per xoo Gms. CHCU.
Ethylamine Hydrochloride C1H6.NH2.HCI 279.9 0.17
Diethylamine " (CjH6)2NH.HCl 231.7 29.45
Hydrobromide (CjUJjNH.HBr 3 11 . 6 46 . 65
Hydroiodide (QJl6)2NH.HI 377.2 71.56
Triethylamine Hydrochloride (CiH6)8N.HCl 137 17-37
Hydrobromide (CjH6)8N.HBr 1 50 . 6 23 . 44
Hydriodide (CiH6)8N.HI 370 92.2
ETHTL BBOIODB CsH^Br.
Solubility in Ether. (Parmentier. 1893.)
t*. — X3*. o. 12. 22.5. 32.
Gms. CaHsBrper 100 gms. Ether 632 561 462 302 253
Solubility of Ethyl Bromide, etc., in Water.
(Rex, 1906.)
Grams per xoo Grams H|0 at:
Dissolved Substance. /•• *
o**. xo*. 2o*. 3o'
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 ^-SS^ 0.540
ETHTL BUTYRATE CiHrCOOCiHs.
SOLUBILCTY IN 'WaTER AND IN AqUEOUS EtHYL AlCOHOL MIXTURES AT 20*.
100 g. HiO dissolve 0.5 g. ethyl butyrate at 22®. (TVaube, 1884.)
100 cc. HsO dissolve 0.8 cc. ethyl butyrate at 20^. (Banaoft, 1895O
100 cc. ethyl butyrate dissolve 0.4 — 0.5 cc. HiO at 20®.
Per 5 CC. (cc. HjO 10 6 4 2.96 2.10
Ethyl Alcohol I cc. CsHtCOOCjHs o . 34 o . 96 2 . 47 4 6
BTHTL CARBAMATE (Urethan) CO(OCsHt)NHt. See also p. 74i.
Solubility in Several Scm-vents at 25®. (u. s. P. vm.)
Solvent. Water. Alcohol. Ether. Chloroform. GlyoeroL
Gms. C»(0C»H6)NH» ) , ,,
per 100 gms. solvent ! '°°+ *^ '~ 77 33
297
ETHTL ETHER
Rbciprocal Solubility up Ethbr and Water.
(KlobUe— Z.phyiik.Chein. Ht 6x91 '97; Sdumdce— 7M4. 14. 334. W. St.ToUoczko— /Mrf.ao»407.
•96.)
Solubility of Ether in Water.
Lower Layer — Aqueous.
, Cms. (C9Hi)iO per 100 Cms.
Solubility of Water in Ether.
Upper Layer — Ethereal.
Cms. HsO per zoo Gms.
• • *—
Water. Solation.
Ether.
Solution.'
0
13.12 II. 6
1. 01
I.O
s
II
.4 10.2 ,
06
I OS
zo
9
5 8.7
.12
1. 12 (2.6, S.)
15
8
2 7.6
.16
115
20
6
95 6.5
20
1.20 (2.65,8.)
25
6
05 5-7
.26
1.36
30
5
4 51
33
I 32
*4o
4
7 45
52
1.50
*5o
4
3 41
73
1-7
*6o
3
8 3-7
83
1.8
♦70
3
3 32
2.
04
2.0
*8o
2.
9 2.8
2
25
2.3
•
•Indie
atesd
theticMc
thod.
for which see pue lA.
100 cc. HsO dissolve 8.1 1 cc. ether at 22°; vol. of solution, 107.145 cc., Sp.
Gr. 0.9853.
100 cc. ether dissolve 2.93 cc H^ at 22^; vol. of solution, 103.282 cc; Sp. Gr.
0.7164. (Hen, 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, 1912a.
Solubility op Ethbr in Aqueous Solutions op Hydrochloric
Acid.
(SchuDcke — Z. physik. Chem. I4c 334, '94; in 38-5^% HO, Draper — Chem. Newa, 35, 87. '77O
In
38Sa %
cc. Ether
HQ. In 31.61 %HC1.
In 30 % HCl.
cc. Ether Gms. per x
Gram HsO.
cc. Ether Gms. per x g. HgO.
t\
per 100 cc
S(dTent.
per too cc. __ _
(CH1O.O.
^^" HQ. (CH.)K>.
-6
181
1.49. 0.4632
I 387
67.2 0253 0.5637
0
I77S
142 0.4622
1.308
58.3 0253 04863
+6
17a S
131. 5 04622
1.2075
51. I 0.253 0.4231
15
163
121.7(14°) 0.4632
I . 1075
40. 5 0.253 0.3299
20
158
III. 9 (20.8°) 04632
1.0005
33^ 0253 0.2688
26
»3S
104.2 0.4622
0.9360
27.5 0.253 0.2221
In 12.58 %HC1.
In 3.65 % HQ.
*0
ccEUwrper Gnu. peri Gram HiO.
cc. Ether per Gms. per 1 Gram HjO.
• •
looec.!
xdvent. HCl. (CjH«)iO.
looccSolmit. HCl. (CiIU)K>.
-6
26
.45 0.144 0.3106
19.23
0.0308 0.1454
0
92
.19 0.144 0.1748
...
... ...
+6
X9
.18 0.144 0.1503
14-31
0.0308 0.1070
«S
15
.6x 0.144 01210
11.83
00308 0.0868
ao
13
.76 0.144 0.1059
10. 52
0.0308 0.0769
36
12
.70 0.144 00970
9.24
0.0308 0.0673
The above data are recalculated and discussed by Jiittner, 1901.
BTH7L BTBEB
298
Data for the solubility of ethyl ether in carbon dioxide at hig^h pressures are
given by Sander (191 1-12). The determinations were made by using c^uite small
amounts of ether and observing the pressure at which a drop oT 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 COti 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 Mcintosh (19 13).
Solubility of Ether in Aqueous Salt, Etc., Solutions at i8^
Aci. Sdu-
tion of:
Water
KNO»
KCl
LiCl
NaCl
Cms. per
Liter Added
Salt.
O
loi . 19
73-6
42.48
58. S
(Euler, i904.)
Gms. (C|Hi)sO
per xoooc.
SolvefkL
7.8
S-4
4.7
4-5
A5]. Solo-
tionof:
Na^SOi
Maimite
H4SO4
ii
Gms. per
Liter Added
Salt.
59-54
91.06
49
122.5
245-
Gins.(C|HO/>
per xoooc
Solvmt.
3-7
6.7
6.6
5 -65
4. 55
Solubility of Ethyl
Solvent.
Water
o.s»NaI
o.5»NaBr
0.5 n NaCl
o.swNaF
o.5»NaiS04
o.SffNatCrO^
o.5»Na«Mo04
o.s»Na«W04
Gms.
(C,H0iO
per zoo cc.
Solvent.
5.8s
S-70
4.68
4.48
4.15
4.30
4.22
4-39
4.12
Solvent.
Ether in Aq. Salt Solutions at 28**.
(Thorin, 19x5.)
Gms.
(CiHO,0
per xoocc
SolvenL
Solvent.
.5»NajP04 4.17
.5f»Na«As04 4.20
.5f»Hg(CN), 5. 71
.S»NH4N0» 5.37
.Sf»FeCIi 5.09
.5»NasCrs07 4.84
.SnFcSOi 4.33
.S»Alj(S04)i 3.9s
o . 5 n Na Succinate
o. 5 nNa Citrate
o. 5 f»Na Acetate
0.5 nNa Tartrate
o . 5 n Na Phthalate
o . 5 n Na Cinnamate
o.5»NaBenzoate
o . 5 n Na Salicylate
Gms.
(C,H,)iO
per xoooc.
Solvent.
4.68
4.19
4. IS
4.12
5.88
6.29
5-99
6.44
o
0.5 » Am. Oxalate 4. 74 o. 5 »Na Benzene Sulfonate 6.05
Solubility op £thyl Ether in 0.91 Per Cent (Physiological Normal
Saline) Aqueous NaCl Solution.
5 by freezing-point method
. Ether of
•
Gms. (C|IIi)sO
^ cc. (QHOiO
f.
per xooGms.
(at X5*) per 100
Aq. Naa.
cc. Aq. NaCL
0
13.08
18.27
5
II. 15
15.58
10
9-45
13.20
IS
8.10
II. 31
20
6.87
9.60
25
S-9<^
^33
30
5-30
7.40
Purified ether prepared from methylated spirit gave slightly higher results.
SOLVBXUTY OF EtHYL EtHER IN Aq. SULFURIC AciD AT O^
(Kitmann, xQxoa.)
Gms. per xoo Gms. Homogeneous Mixture. Gms. per xoo Gms. Homogeneous Mixture. '
(C.H^«0.
H«0.
H,S04.
' (CHOA
H,0.
H«S04.
24.2
34.5
41.3
16. 1
42.7
41.2
24.8
35-4
39.8
6.1
78
159
43.9
15-7
40.4
53-8
8.5
37.7
34
26.1
39-9
Data for the system ethyl ether, ethyl alcohol, water, sulfuric acid at o® are also
given.
299 BTHYL
SoLUBn^mr op Ethbs in Aqueous Ethyl Alcohol and in Aqueous
Methyl Alcohol Mixtures at 20®.
(BancioCt, 1895.)
In Ethyl Alcohol.
In Methyl Alcohol.
Per sec
. C,H»0H.
Per 5 cc CAOH.
Per X cc. CHiOH.
oc H^. cc. (QIIi)s0l
Per X cc. CH/)H.
ccHiO.'
cc.(CA)*0.t
ccHrf).* ce.
(CA)Af
cc. HiO. cc. (C,H»)^
SO
1.30
4 -45
7
ID
113
0.83 1.80
25
1.70
4
7.8
7
0.8s
0.64 3
10
2.41
3.87
8
4
0.60
0.52 S
8
3-3S
3.10
10
2.S
0.56
0.44 10
6
S-io
2.08
IS
1.8
0.63
0-4S IS
S-2I
6
1.77
17s
I
1.23
* Saturated with ether.
t Saturated with water.
((
M
tt
U
€€
U
The System Ethyl Ether-Malonic Aqd-Water at 15**. (KlobUe. 1897*)
Results for Conjugated Liquid Layers Formed Results for the Liouid Layers in
when Insufficient Malonic Acid to Satu- Contact with Excess of
rate the Solutions Was Present. Malonic Acid.
Oaa. per xoo Gms. Lower Gms. per xoo Gms. Upper Gnu. per xoo Gmi.
W«' , . .^y^' - ^P^- SolidPhMe.
Malonk t7^ Ethyl Maloiuc n rw Ethyl Malonic n r\ Ethyl.
Add. **^- Ether. Add. "«^' Ether. Add. "^- Ether.
o 92.23 7.77 o 1.20 98.80 8 o 92 Malonic Acid
4.63 87.42 7.94 0.72 1.54 97.74 9.96 0.42 89.61
11.60 79.92 8.48 2.19 1.99 95.82 19.41 2.79 77.80
20.45 69.55 9.99 5.01 3.08 91.91 27.22 5.23 67.54
27.43 60.57 12 9.52 5.19 85.29 35.51 10.73 5375
33-^3 47-45 18.80 21.89 ^3-4^ 64.91 46.48 20.86 32.66 **
34.17 35.81 30.02 30.44 25.37 44.19 51-33 26.30 22.36
31. II 26.76 42.12 31. II 26.76 42.12 57.37 39.10 3.52
Data for the system ethyl ether, succinic acid nitrile and water are given
by Schreinemakers, i8p8.
Data for the extraction of formic acid from water by ether are given by Dakin,
Janney and Wakemann, 1913.
ETHTL rOBlCATE HCOOCHs.
100 grams water dissolve 10 grams ethyl formate at 22^ (JmaSa^ iSM
KTHTL METHYL KETONE CHi.CO.CsHs.
Solubility in^Water. (Rothmund; 1898.)
By synthetic method, see Note, page 16.
^ Gms. Ketone per loo Gms. ^ Gms. Ketone per loo Gms.
Aq. Layer. Ketone Layer. * Aq. Layer. Ketone Layer.
— 10 34.5 89.7 90 16. 1 84.8
+10 26.1 90 iio 17.7 80
30 21.9 89.9 130 21.8 71.9
SO 17.5 89 140 26 64
70 16.2 85.7 i5i.8(crit.temp.)44.2
The accuracy of Rothmund's data is questioned by Marshall (1906) and the
following new determinations given.
v. 64.7'. 6s. S*. 73. 6*. 91. o*. IS*. 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
1-5% 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 (191 1) and by Bruni, 1899, 1900.
ETHTL KBTOm 300
DiBTHTL KBTONS (Propione) (CtH»),CO.
S(X.UBILITY IN Water. (ReUummd. 1898.)
The detetmiiiatioiis were made by Synthetic Method, see p. 16. The
temperature could not be reached and high accuracy is not ckumed for the results.
Gm. Dktliyl Ketone Gm. Dietbyi Ketone
f», per loo Gma. f», per 100 Gnu.
Aq. Layer. Ketone Layer. Aq. Layer. Ketone Layer.
20 4.60 ... 100 3.68 93.10
40 3-43 97-42 120 4.05 90.18
60 3.08 96.18 140 4.76 87.01
80 3.20 94.92 160 6.10 83.33
ETHYL PROPIONATE CtH.COOCsH».
Solubility in Watbr and in Aqueous Ethyl Alcohol Mecturbs.
(Pfeiller, 1892; Bancroft, 189s.)
^ At..,,^^ oc H/) to Cause Sepaxatkm of a Second Phase in
Sf'wlS^ Ifibctmcs of tbeGtvesi Amounts of Alcohol
inMiztue. and 3 cc Portions of Ethyl Propionate.
3 2 32
6 6.87
9 12.3s
12 19.17
IS 27.12
18 36.84
21 50.42
24 00
100 grama H|0 dissolve 1.7 grams ethyl propionate at 22^ CTranbe, Z884O
DiETHTL Diacetyl TA&T&ATE (CHOCOCH,)t(COOCtH«)i.
Freezinp;-point lowering data (solubility, see footnote, p. i) for mixtures of
diethyl diacetvl tartrate and each of the following compounds are given by
Scheuer (19 10); m nitrotoluene, ethylene bromide, phenol and naphthalene.
Results for diethyl diacetyl tartrate and naphthalene are also given by Palazzo
and Batelli (1883).
ETHTL VALERATE QHiCOOQHt.
ETHYL (Iso) VALERATE (CH,)t.CH.CHaCOOCsHf.
Solubility op Each in Water and in Aqueous Alcohol Mixtures at 20^
(PfeiSer. 1893; Bancreft, 189SO
TOO CO. water dissolve 0.3 cc. ethyl valerate at 25^.
100 cc. water dissolve 0.2 cc. ethyl iso valerate at 20**.
100 cc. ethyl iso valerate dissolve 0.4+ cc. water at 20®.
Mixtures of Ethyl Alcohol, Mixttires of Ethyl Alcohol,
Ethyl Valerate and Water. Ethyl Iso Valerate and Water.
IVr 5 cc. Ethyl Alcohol.
oc Alcohol.*
ccHaO.t
ccAlmhnl.*
oc.H|0.t
ccHsO.
cc. Ethyl
laoValcxatc.
3
1.42
39
S3 '^3
9
7.18
45
63.60
10
0.15
IS
14-13
57
9053
8
0.23
21
22.40
72
131. 0
6
0.46
27
31-62
81
180.0
5.
0.72
33
41.63
4
1.23
* oe. Alcohid in mixture.
cc HfO added to cause
3 cc. portiook of ethyl valerate.
t cc HfO added to oiuse the separation of a second phase in nizturcs of the given amomita of alcohol
301
^vU' soLUBKurr in Water and in Alcohol.
r.
0
0.
0.226
0.0281
Solubility in AkohoL
5
0.191
0.0237
f.
no YdTAkolnL
10
0.162
0.0200
0
3S9S
IS
0.139
O.OI7I
4
337 S
20
0.122
0.0150
10
308.6
25
0.108
0,0131
IS
288.9
30
0.098
O.OII8
20
«7i.3
For fi and q see Ethane, p. 285.
SOLUBILITT OF EtHTLBNB IN AqUBOUS SOLUTIONS OF AlKAU HTIttOZmi%
Etc., at I5^ (BiUitaer, tSoaO
Results in terms of the Ostwald Solubility Expression L See p. 237.
AqoNOi Solution of : /-
Solubility (u in Aq. Sohitk» of NonnaHty:
0.1. o>»S' 0.5. a7S< 1,0.
KOH 0.154 0.144 0.130 0.118 0.1056
NaOH 0.153 0.144 0.128 0.114 o.ioi
NH«OH ... 0.157 0.156 0.155 0.154
}Na«S04 0,1525 0.1425 0.127 0.109 0.093
In H|0 alone 0.1593
Solubility op Ethylene in Mbthyl Alcohol and in Acetonb. (Uvi, 19014
Results in terms of the Ostwald Solubility Expression L See p. 227*
f*. In Methyl Alcohol. In Acetone. I*. In Methyl Alcohol. In Acetone.
o 3 3924 40652 30 1.8585 1.8680
10 2.8831 3-3580 40 I.343* 1.0852
20 2.3718 2.6278 50 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, ^ = 3 3924 — 0.05083 / — o.ooooi fl.
In Acetone, I = 4.0652 — 0.06946/ — 0.000126 ^,
Solubility of Ethylene in Several Solvents. (McDanJei, ign.)
Abe. Coef. Bunien c««Ivm«* *• Abe. Coef. Buniw
A. Coef./I. Solvent. t. ^ ^,^^
3.010 2.786 Heptane aa.4 3.463 ^.zoj
3.655 3-353 " 35 3' 186 a.8a4
3.482 3.100 ** 39 . 3. no a.7aa
3.038 3.8141 Acetone ao a. 571 3.390
a. 826 3.505 " 35 3.308 3.046
3.586 2.219 Limonene 33 no constant equilibrium
vol. of ethylene absorbed by unit vol. of solvent at temp, statedt
For definition of Bunsen Coef. /8, see carbon dioxide, p. 227.
The Coef. of Abs. fi of ethylene in Russian petroleum is 0. i64at 10* and o. 142 at 20*.
(Oniewoes and WaUit, i8S7')
Freezine-point data (solubility, see footnote, p. i) for mixtures of ethylene and
methyl ether are given by Baume and Germann, 191 1, 1914*
ETHTLENB BROIODB CtH4Brt.
F.-PT. Data for Mixtures of Ethylene Bromidb and Other Coiipoundb.
Ethylene Bromide + Naphthalene (Baud, xgxi ; Dtbme, 1895.)
+ /? Naphthol (Bnini, iW)
-f '* + Picric Acid (Bnml, X898.)
-f Paraldehyde (Pateno tnd AmpoU, 1897.)
•f Phenol (Dahms, 1895; Pateno and Ampob, 1^97^
+ Toluene (Baud, 1913.)
-f Bromotoluene (Pateno and Ampda, 1897.)
+ ^ Xylene ** ••
Solvent.
r.
Benzene
33
Hezane
35
50
33
35
f 45
Abs. Coef. A
£A •
M
ETHTLENB CTANIDB
302
ETHTLENB CTANIDB C,H4(CN)t.
Distribution Between Water and Chloroform. (Hantach tnd Vagt, 1901.)
Gm. Mds. CH<(CN), per Liter. . £j.
Aq. Layer, Ci. CHCU Layer,' c^. ' c^
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, KCl and HCl on the above distri-
bution are also given.
DiETHTLENE ETHER (CH/)CHs)t.
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
diethylene ether and water, by Unkovskaja, 19 13.
}
Tetraphenyl ETHTLENB (CcHt)sC:C(C«H»)s.
Freezing-point data for tetraphenyl ethylene -f silicotetraphenyl are given by
Pascal and Normand (1913).
0 BUCAINB CuHuNOt and Salts.
100 cc. HtO dissolve 0.296 gm. anhydrous fi eucaine at 20^.
100 cc. oil of sesame dissolve 3.49 gms. anhydrous fi eucaine at 20**.
100 cc. aniline oil dissolve 66.6 gms. anhydrous fi eucaine at 20°.
100 cc. HsO dissolve 2.5 gms./9 eucaine hydrochloride at 15-20*
100 cc. 00% alcohol " 9 " " "
100 cc. HsO " 25 " " lactate
100 cc. 90% alcohol " 12.5
100 cc. CHCU " 20
EUROPIUM Bromonitrobenzene SULFONATE Eu[C«H,Br(i)N0t(4)S0t(2)]a.-
loHsO.
100 gms. sat. solution in water contain 6.31 gms. anhydrous salt at 2^^
(Katz and James, 1913.)
VATS.
Solubility of the Fatty Acids Obtained from Several Sources in
Alcohol and in Benzene. (Dubois and Fade. 1885.)
41
II
II
II
II
II
II
II
II
II
11
(Zalai.
19x0.)
(Squire and
Caines,
1905.)
Crude Fatty
Add of:
Mutton
Beef
Veal
Pork
Butter
Maigarine
Gms. Fat per xoo Gms. Abs. Alcohol at:
o'.
2.48
5
S.63
10.61
2.37
IO-.
S.02
6.05
13.78
11.23
24.81
4.94
26\
67.96
82.23
137.10
118.98
158.2
47.06
Gms. Fats per xoo
Gma. Benzene at xs^
14.70
15-89
26.08
27.30
69.61
13.53
Miscibility OF Fats and 90 Vol. Per Cent Alcohol at 37®. (Vandeveide. 19x1^
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- Volume after AgiUtion. Gms. Fat per Gms. Alcohol
— --I2Z: — * ^— — — . ' ^ — . 100 Gms. per xoo Gma.
cc. Alcohol ccFat Alcohol Layer Fat Layer.
cc. Alcohol
Alcohol + Cocaline 25
« " 20
« «
« u
15
10
5
Alcohol + Butter Fat 25
" " 20
15
10
5
25
20
15
10
5
it
It
tt
it
it
Alcohol + OUve OU
(( tt
tt
tt
tt
u
tt
tt
cc. Fat
5
10
IS
20
25
5
10
IS
20
25
5
10
15
20
25
25.4
19.2
13
6.7
I.I
25.1
19.2
13
7.1
2
24.7
19.2
13
7-5
2.2
4.6
10.8
17
23.3
28.9
4 9
10.8
17
22.9
28
5.3
10.8
17
22.5
27.8
4
5
7
9
13
3
3
4
5
14
2
2
2
3
7
9
6
2
I
5
5
7
I
3
4
4
5
19.4
16.2
13. 5
12.2
II. 4
174
14. 1
14. 1
II. 4
95
11. 2
8.7
8.7
8.8
y.6
For other data on the solubility of fats see Ewers (1910) and Louise (1911).
303 nnoRunB
nUORUnB (Diphenylenemethane) C«H4.CHt.CfH4.
Freezing-point data (solubility, see footnote, p. i) are given by Kremann (191 1 J
for mixtures of fluorene and each of the following compounds: o, m and p dintro-
benzene, i.3.5» trinitrobenzene, dinitrophenol, dmitrotoluene, trinitrotoluene and
picric add.
nUOBESCEIN CsDHuOk.
100 gms. H2O dissolve 0.005 fi^- fluorescein at 20-25® (Defan. 19x70
100 gms. pyridine dissolve 13.29 gms. fluorescein at 20-25** '*
100 gms. aq. 50% pyridine dissolve 37.22 gms. fluorescein at 20-25® "
rOBMALDEHTDB, SoUd Polymers (CHsO)».
Solubility of the Six Well-Dbfined Solid Polymers of Formal-
dehyde IN Water. (Auerbach tnd Banchall, 1908.)
Name. Formula. m. pt. Gms. per xoo cc. Sat. Solution in Water.
Parafoimaldehyde (CHsO)n+^HiO 150-160 20-30 gms. at 18®
a Poljroxymethylene (CHsO)n 163-8 11 gms. at 18-25®
fi Polyoxymethylene (CHsO)f| 163-8 3.3 gms. at 18®, about 4 at 25®
7 Polyoxymethylene (CHsO)^ i63~5 less than o.i at 18®. 0.1 gm. at 25®
i Poljroxymethvlene (CHsO),» 169-70 practically insoluble
a Triozymethyfene CiHcQi 63-4 17.2 at 18®, 21.x at 25®
All are insoluble in alcohol and ether except trioxymethylene.
Solubility of Trioxymethylene in Aq. Sodium Sulfite S(».utions at 15®.
(Lumite and Sorewetz, 1902.)
Gms. Na^SOs 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 20®. (Hantach and Vagt, 190Z.)
yORMAMTDB HCONHt.
Solubility in Water, Determined by the Freezing-point Method.
(Enjciish and Turner, 1915.)
Gms. Gms. Gms.
SA ^^^^ Solid rojt HCONH, Solid Ph«e. S^., HCONHi SofidPhM*
Solidit. per 100 Phase. Soiidif. per 100 ^'*'"" xruamu Solidif. per xoo ^^
Gms. H|0. Gms. H|0. Gms. H|0.
— 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 " -454 187.8 HCONHj.HjO -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 +
propionic add.
oandp ChloroFOBMANIUDBS Ci.COI^NH.CHO.
Freezing-point lowering data for mixtures of 0 and p chloroformanilide are
given by Rmg and Orton, 191 1.
rOBMIC ACID HCOOH.
Solubility in Water, Determined by Freezing-point Method. (Faucon, X910O
M ^ Gms. HCOOH
t^ nf
Gms. HCOOH
t*'of
Gna.HCOOK
SoMif. '^STuSr
w 01
Solidif.
per xoo Gms.
Mixture.
Solidif.
per xoo Gms.
Mixture.
0 0
-30
53
-40
74.2
-S ".s
-35
57-6
-30
79
-10 23
-40
62.5
— 20
84.3
-IS 32
-45
66.S
— 10
89.4
—20 39.2
—49 Eutec.
70
0
95
-25 46. S
-45
71.7
+8.51
100
Similar data for mixtures of 97.4% formic acid and water are given by Kremann,
1907.
rasMic AOiD 304
Distribution op Formic Acm Between Water and Benzene at 13-15^
(v. Geoigievics, 19x3.)
A small separatory funnel was used and the acid in each layer titrated with o.x
n NaOH, using phenolphthaleine as indicator.
Gmft. HCXX)H Found per: Gms. HCXX)H Found per:
% / -^ \
25 oc. H|0 Layer. 150 ocC^ Layer. 95 cc B|0 Layer. 150 ccCA Layer.
1. 016 0.016 2.365 o.o^s
1. 539 0.031 3.826 0.062
1.800 0.024 5-874 0.II4
2. 112 0.031 ^ 7-836 0.138
The distribution ratio of formic add between water and benzene was found by
King and Narracott (1^09) 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.
rUMABIC ACID COOH.CH:CH.COOH.
IIALEIC ACID COOH.CH:CH.COOH. (See also p. 398.)
Solubility in Water. (Vaubd, 1899.)
100 gms. water dissolve 0.672 gm. fumaric acid at 165^
100 gms. water dissolve 50 erams maleic acid at loo^
Data for the distribution of fumaric acid between water and ether at 25^ are
given by Chandler, 1908.
irBFUBOL QHiOCHO.
Solubility in Water. (Rothmund, 1898.)
Determinations by Synthetic Method, for which see p. 16.
Gms. CJI^OCHO per loo Gms. . . Gms. C4H/)CH0 per 100 Gms.
» .
Aq. Layer.
FuHuzol Layer.
» .
Aq. Layer. Furfurol Layer
40
8.2
93-7
100
18.9 83.5
so
8.6
93
1 10
24 78. s
60
9.2
92
"5
28 74.6
70
10.8
90.7
120
34.4 68.1
80
13
89
122.7
(crit. t.) SI
90
iSS
86.6
GADOLINIUM CobaltiCTANIDB Gdt(CoC«N.)s.9HiO.
1000 gms. aq. 10% hydrochloric acid dissolve 1.86 gms. of the salt at 25^.
Guoes and Wfllaid, 19x6.)
GADOLINIUM GLTCOLATE Gdt(C,H,0,),.2H,0.
1000 cc. HtO dissolve 14.147 gms. of the salt at 20^. (Jantach and GrOnknutt, Z9xs-i3-)
GADOLINIUM Magnesium NTTBATE, etc.
Solubility of Double Nitrates of Gadolinium and Other Metals in Conc.
Nitric Acid of tfy - 1.325 (-51.59 Gm. HNOi per 100 cc.) at I6^ jantsch, z9xa.)
Gms. Hydrcted
Salt. Formula. Salt per Liter
SaL SolutKMk.
Gadolinium Magnesium Nitrate lGd(NO8)6]sMgs.24H«0 352 .3
" Nickel " " Nia " 400.8
Cobalt " " Co, " 4Si-4
" Zinc " " Zm " 472.7
GADOLINIUM OXALATE Gd,(C,04),.ioH/).
Solubility in Aqueous Solutions of Sulfuric Aero at 25*. (Wkth, 1913.)
Solid Phase.
Gds(CsO4)s.ioHa0
u
ii
a
Normality of
Gms. per loo C
[jms. Sat. Sol.
Aq.^SOi.
G<iA.
Gd,(C04),.
2.16
0.1883
0.3005
3"
0.3010
0.4803
432
0.43S9
0.6956
6.17s
0.707
1. 128
305 QADOLINIUM OZALATK
Solubility of Gadolinium Oxalate in Aqueous 20% Solutions of
Mbthylamine Oxalate, Ethylaminb Oxalate and Triethylamine Oxalate.
(Grant and James, X9z7«)
Solvent. ^ ^Too^^^r
Aq. 20% Methylamine Oxalate 0.069
" Ethylamine " 0.360
" Triethylamine " 0.883
aXDOUNIXTM Dimethyl PHOSPHATE Gds[(CH.),P04]«.
100 gms. HaO dissolve 23 gms. Gds[(CHs)iP04]6 at 25^ and 6.7 gms. at 95^
(Moxxan and James. 1914.)
aADOUNIXTM SULFATE GdiCSOOi-SHtO.
Solubility in Water. (Benedicks, 1900.)
*••/ ^""'^^^^'^ Sdid Phase.
o 3 . 98 ' Gdi(S04)«.8HiO
10 3-3 "
14 2.8 "
25 2.4 "
34.4 2.26 "
Solubility of Gaikx^inium Sulfate in Aqueous Solutions of:
Sodium Sulfate at 25% (Bissell and James, 19x6.) Sulfuric Acid at 25^ (Wirth, z9za.}
Gms. per lop Gms. HA « .„ p. ^ NonnaUty Gms. per loo Gms. Sat. Sol.
' Na^,. Gd.(S0^,.' Sohd Phase. ofH,So/ ' QdA - Gd.(SO0,. ^ ^obd Phase,
o 2.15 Gds(S04)t.8HaO o 1.793 3- 9^1 Gda(SO0t.8H/)
0.43 2.06 " 0.1 1.98 3-291 "
0.47 0.76 Gds(S04)s.NatS04.2HsO 0.505 2.365 3.931 "
1.26 0.17 " I.I 2.29 3.807 "
3.01 0.07 " 2.16 1.789 2.974 "
7.46 0.05 " 6.175 0.528 0.8777 "
27.40 0.05 " 12.6 0.0521 0.0867 **
aADOUNIXTM SULFONATES.
Solubility in Water. ^^^^
Salt. Formula. *'&at?!j5S Authority.
Gm8.H/).
^tTsSfoS !Gd[C.H.(NO0SO.].7HW „ 43-8 j '^^'
"^Se^sS^U i G<llCaBr(NQ0SQ.(x^.«)VxoaO ,5 6.3. j ,^;^,
GALACTOSE CeHitOs. See also Suggars, pages 695-7.
100 gms. saturated solution in pyridine contain 5.45 gms. QHisOe at 26^,
density of solution » 1.0065. (Holty, 1905.)
100 gms. HiO dissolve 68.3 gms. galactose at 20-25^. (Defan, 9x7.)
100 gms. aq. 50% pyridine dissolve 6.83 gms. galactose at 20-25^ "
QALUC ACm 3.4.5, (OH)iC6H,COOH.HtO.
Solubility in Aqueous Ethyl Alcohol at 25®.
(Seiddl, 19x0.)
Sat. Sol. solvent. gat. SoL
1. 15 60 0.957 16
2 70 0.946 18
4.2 80 0.933 19.9
7.5 90 0.919 21.2
10.6 95 O.9II 21.6
13.4 100 0.902 22.2
100 gms. HaO dissolve 0.95 gm. gallic add at 15^. ((keenish and Smith, x9q3.)
100 gms. HtO dissolve 33. 3 gms. gallic acid at loo^ (U. S. P. vm)
Wt. Per Cent
CAOHin
Solvent.
dWofSat.S
0
1.002
10
0.992
20
0.983
30
0.977
40
0.972
SO
0.965
QALUC ACm 306
Solubility of Gallic Acid in Organic Solvents at 2$\
(Seidell, 19x0.)
• A. /*f «?-♦ Gmi. &Hi(0H)t
Solvent. Density of Solvent. &4utSn.* C00H.BW) per 100
Gms. Sat. Sol.
Acetone Jis = o. 797 o . 941 25 . 99
Amylalcohol (iso) djo = 0.817 0.834 5.39
Amylacetate <^ = 0.875 0.878 2.72
Benzene dn = c.873 0.875 0.022
Carbon Disulfide (^=1.258 1.262 0.042
Ether (abs.) d^} = 0.711 0.718 i-37o
Ethylacetate (^ = 0.892 0.911 3.610
The amount of gallic acid dissolved by carbon tetrachloride, chloroform and
toluene was too small for -estimation.
•
100 g:ms. glycerol dissolve 8.3 gms. C«Ha(OH)tCOOH.HiO at 25*. (U. S. P. vm.)
100 gms. 95% formic acid dissolve 0.56 gm. gallic acid at]i9.4^ (Aachan, 19x3.)
aSBMANIXJM DIOXIDE GeO..
100 gms. HiO dissolve 0.405 gm. GeOt at 20^, and 1.07 gms. at loo^ (Winkler, 1887.)
aSBMANIXJM (Mono) SULFIDE GeS
GEBMANIXJM (Di) SX7LFIDE GeSt.
100 gms. HtO dissolve 0.24 gm. GeS
100 gms. HiO dissolve 0.45 gm. GeSt. C^nUer, 1887.)
GLASS.
For data on the solubility of glass in water and other solvents, see:
(Cowper, x88a; Emmerling, X869; BGhling, 1884; Kreasler and Henhold, X884; Kohliauich, 1891;
FGister, x89a; Mylius and FOrster, 1889; x89a; Wartha, 1885; Nicolaidot, X9x6.)
QLOBUUN (Serum).
Solubility in Aqueous Magnesium Sulfate Sch^utions.
(Galeotti, X906; Scaffidi, 1907.)
The precipitated globulin (from oxblood) was not dried, but pressed between
filter paper, and an excess introduced into each MgS04 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 S0«
and dried and weighed.
Results for I0^ Results for 25®. Results for 40®. Results'for 55®. Results for 70*.
Gms. per i<fo Gms. Gms. per xoo Gms. Gms. per xoo Gms. Gms. per 100 Gms. Gms. per xoo Gms.
Sat. Sol. Sat.Sol. Sat. Sol. Sat. Sol. Sat. Sol.
MgS04. Globulin.' MgSO^. Globulus 'MgSOi. Globulin. ^ylgSOi. Globulin.' MgSOi. Globulin.'
0.06 0.07 0.06 0.07 0.06 0.42 0.40 1. 14 0.71 0.34
0.18 0.34 0.21 0.61 0.31 1.42 0.88 2.14 2.52 0.55
0.65 1.63 0.63 2.20 0.61 S.39 1.60 3.34 4.74 1. 14
2. II 3.3s 2.28 5.56 1.92 8.31 S.64 5.06 6.83 1. 17
4.32 4.42 3.3s 6.07 5.40 8.63 10.81 3.10 9.22 1.76
13.63 2.60 16 4.03 14.72 3 13-84 2. II 13.29 I
20.86 0.37 21.30 0.9s 18.47 I-02 1790 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.
QLUCOSE d C«Hii06.HtO. See also Sugars, pages 695-7.
100 gms. HiO ' dissolve 82 gms. glucose at 20-25^ (Defan, 19x7.)
100 gms. pyridine " 7.62 " " " ••
100 gms. aq. 50% pyridine " 4917 " " " **
100 gms. tnchlor ethylene " 0.006 ** " 15*
(Wester and Bruins, 19x4.)
GLUTAMINIC ACID C,H,NH,(COOH),.
Data for the solubility of glutaminic acid in aq. salt solutions are given by
WQrgler (1914) and Pfeiffer and WUrgler (1916).
r.
Gms. GluUminic Add
HCl per xoo oc.
Sat. Sol.
o
3^'S
lO
20
34. S
38
30
42. s
40
47
SO
S2
307 GLUTAMINIC ACID
QLUTAMINIG ACID H7DBOCHLOBIDE C.HiNHi(COOH)t.HCL
Solubility in Water. (Stoiuenberg, 19x9.)
(The following results were taken from the diagram given by the author.)
Gms. Glutaminic Add.
t*. HQ per zoo oc.
Sat.S6L
60 S7
70 62
80 67.5
90 74
icx> 81
20 1.4 (sol. sat. with HQ)
GLUTABIC ACm (Pyrotartaric) (CHs),(COOH)s.
Solubility in Water. (Lamourouz, 1899)
t*. o'. IS*. ao*. 3S*. so*. 6s'.
Gms. (CH,),(C00H)2
I>er ICO cc. solution 42.9 58.7 63.9 79.7 95.7 111.8
ibo gms. 9s % formic acid dissolve 55.62 p^ms. glutaric acid at 18.6^. (Aaduui, X9X3.)
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, 19144
QLYCINE (Glycocoll) CH,.NH,.COOH.
100 gms. HjO dissolve 51 gms. CHi.NHj.COOH at 20-25®. (Dehn, 19x7.)
100 gms. pyridine dissolve 0.61 gm. CHj.NHj.COOH at 20-25*. "
100 gms. aq. 50% pyridine dissolve 0.74 gm. CH1.NH1.COOH at.20-25^ "
Solubility of GLYaNE in Water and in Aq. Salt Solutions at 20^
(Pfdfier and Wttrgler, 191 s, 19x6.)
Mol8.Salt ^!^??y?^ C.U Mob. Salt ^"^9!^^
Salt.
petUter.
per xocc
Sat. Sol.
Water
only
1.962
BaCls
o-S
2.37s
BaBra
o-S
2-954
SrCU
o-S
2.362
SrBra
0.49
2.440
CaCl,
057
4.848
CaBr,
.0.51
4.994
Salt.
per
Liter.
per locc.
Sat. Sol.
LiCl
0
.96
4.188
UBr
0
97
4-245
SrCI,
0
•25
2.129
((
0
•SO
2.331
MM
I
2. 60s
a
2
3 301
10 cc. sat. aq. solution contains 1.8 gms. glycine + 2.7 gms. KCl at 20® when
both are present in the solid phase. (Pfeiffer and Modebki. 19x9.)
GLYCOUC ACID CH,OH.COOH.
_ Solubility in Water. (Emidi, 1884.)
^ t*. 30*. 6o*. 8o*. xoo*.
Gms. CH20H(C00H)
per 100 gms. HsO 0.033 0.102 0.235 0.850
PhenyiaLYCOUC ACID dextro and racemic CH.C«H».OH.COOH.
Solubility of Dextro and of Racemic Phenyl Glycolic Acm in Chloroform.
(HoUeinan, 1898.)
Gms. Detro Add Gms. Racemic
t*. per 100 Gma. t*. Add per xoo
CHCU. Gms. CHOs.
15 0-952 15 0.877
25 1.328 25 1.07
35 1-950 35 1.60
QLYCYRRHTZTC ACID.
100 gms. sat. solution in HiO contain 0.575 gm.glycyerrhizic acid at 15^ (Capin,'x9.)
100 gms. sat. solution in HiO contain 0.152 gm. Am. glycyrrhizate at o^ and
0.225 gm. at 15*. ^ (Capin, 191a.)
PhenylGLYOXAL Phenyl hydrazone C«H».CO.CH.N.NH.CsH».
One liter CsHs dissolves 52.6 gms. of the A form at 5^ (Sidgwick, x9xs )
One liter CsHs dissolves 2.9 gms. of the B form at 5^. *«
GOLD 308
GOLD Au.
Solubility of Gold in Potassium Cyanide Solutions. (Msdtitriii, 1893^
Gold disks were placed in Nessler tubes with aqueous KCN solutions.
Gma. Au Dissolved in 34 Hours in Nessler Tubes:
Percent t * \
I * ««. Passed m. AgiUtion.
O.I 0.00195 0.00331
I 0.00162 0.00418 0.00845 0.0187
5 0.0032 0.0046 0.01355 0.0472
20 0.0012 0.00305 O.OII5 0.0314
50 0.00043 0.00026 0.00505 0.0108
The following data for more dilute KCN solutions are given by Christy (looi).
Gold strips 2 X i inch were rotated for 24 hrs. in aq. KCN solutions and the
loss in weight determined.
' 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 o.ia-0.23 0.004 4:^9 0.065 168.12
0.0016 0.16 0.008 48.43
Data are also given for 48 hour periods and for solutions containing Ot.
One liter of cone. HNOs dissolved 0.66 ^m. Auon boiling for two hours. (Dewey, '10.)
Data for the rate and limit of solubility of Au in cone. HCl solutions of iron
alum and of cupric chloride are given by McCaughey, 1909.
GOLD CHLORIDE (Auric) AuCU.
100 gms. HtO dissolve 68 gms. AuCIs.
When I gm. of gold as chloride is dissolved in aq. HCl of different strengths and
the solutions shaken with 100 cc. portions of ether, the following percentages of
thegold enter the ethereal layer. With 20% HCl, 95%; 10% HCl, 98%; 5% HCl,
98%; 11% HCl, 84% and 0.18% HCl, 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 (Aureus) AuaPQ,.
zoo gms. PCla dissolve i gram at 15^, and about 12.5 grams at 120^.
(Lindet — Compt. rend, zoi, 149a, "Ss.)
GOLD ALKALI DOXTBLE CBLORIDBS.
Solubility op Sodium CtOld Chloride, Lithium (jold CHLORiDBt
Potassium Ctold Chloride, Rubidium (3old Chloride, and
Caesium Gold Chloride in Water.
(Roaenbladt — Bcr. X9» »537, '86.)
t*
Grams Anhydrous
Salt per xoo
Grams Solution.
• •
NaAuCU.
liAuCU.
KAuCU.
RbAuCU.
CaAuCU.
10
58 -2
53-1
27.7
4.6
0.5
20
60.2
57-7
38.2
9.0
08
30
64.0
62.5
48.7
13 -4
1-7
40
69.4
67 -3
59-2
17.7
3-2
so
77-5
72.0
70.0
22.2
S-4
60
90.0
76.4
80.2
26.6
8.2
70
• • •
81.0
• • •
31 0
12.0
80
• • •
85 -7
• • •
35-3
16.3
90
• « •
• • •
• • •
39-7
21.7
100
• • •
V • •
• • •
44-2
27 5
100 gms. glycerol (({u ■- 1.256) dissolve 0.21 gm. AuK(CN)i*5HsO at iK-ld^.
(OssendowBkC 1907 )
309 QUAIACOL
QUAIACOL CJi«(OH)OCH,0.
GUAIACOL CABBOKATE [C6H4(OCH,}0]sCO.
Solubility in Water, Alcohol, Etc. (U. s. p. vm.)
Cfj«Mn*
t*
Gms. per
zoo Gms. Solvent.
OatVCIMa
w .
Guaiacol.
Water
25
1.89
...
Alcohol
as
. ■ •
3.0S
Chloroform
2S
...
66.6
Ether
2S
. . •
7.69
Glycerol
2S
100
• a •
The coefficient of distribution of guaiacol carbonate between olive oil and water
at 25® is given as -^ «= 3.7 by BoSseken and Waterman, 191 1, 1912.
Freezing-point lowering data (solubility, see footnote, p. i) are given for mix-
tures of guaiacol and a naphthylamine by Pushin and Mazarovic, 1914J 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 C«H»N:C(NHC6H0i.
Solubility in Mixtures of Alcohol and Water at 25^ (Honemanand Antuacii/94)
GiDS. Gms.
Vol. % CAN:C(NHCA)s Density Vol. % CAN:C(NHCA)s Density
Akohol. per xoo Gms. of Solutions. Alcohol. per xoo Gms. . of SduticMis.
Solvent. Solvent.
100
6.23
0.8021
80
1.06
0.8572
95
3-7S
0.8158
7S
0.67
0.8704
90
2.38
0.8309
70
0.48
0.8828
^S
1.58
0.8433
. 60
0.22
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, 19 13.
HEMOGLOBIN.
100 gms. HsO dissolve 15.16 gms. hemoglobin at 20-25^ (Defan, 19x7.)
100 gms. pyridine dissolve 0.15 gm. hemoglobin at 20-25^ "
100 gms. aq. 50% pyridine dissolve 0.77 gms. hemoglobin at 20-25^ **
HELIANTHIN (Methyl Orange, Tropaeolin).
100 cc. HiO dissolve 0.0055 to 0.0225 S^m. helianthin. (Dehn, x9z7a.)
100 cc. pyridine dissolve 0.^5 gm. helianthin. **
100 cc. 50% aq. pyridine dissolve 62.5 ^s, helianthin. "
Results for other solvents and observations on the state of colored compounds
in solution are given.
He.
SoLUBiLrrv in Water, (von Antropoff. xgog-xo)
f.
Coef . of Absoxption.
0
0.0134
10
O.OIOO
20
30
0.0138
O.O161
40
so
O.OI9I
0.0226
The coef. of absorption adopted for the present results is that of Bunsen aa
modified by Kuenen. The modification consists in substituting unit of mass in
place of unit of volume of water, in the formula.
310
BKUUM He.
Solubility in Water.
(EfltRicher— Z. phyaik. Chem. 31. X84, '99.)
AbsorpCioo Cocffidoit*
••J
Cor.Btnmctie Vol
.at
Vol.o(
JB
'At Bar. Pressure
» . — ^.^^^
PmraiCa
Water.
He.
»•
MimisHiO
Vapor Tensioa.
Pressure*
0
• • •
• • a
• • •
0.000270
• • •
0.0150
OS
764.0
73-584
1.093
«
• * •
0.0149
0-0149
5
758.0
73
■578
1.062
0.000260
0.0144
00146
10
758.0
73
597
1.046
0.00025s
0.0142
0.0144
15
757-8
73
.641
1.008
0.000246
0.0137
00140
30
758 -4
73
.707
0996
0.000242
0.0135
0.0139
25
762.3
73
793
0.983
0.000238
0.0133
0.0137
30
764.4
73
897
0.985
0.000238
0.0133
0.0138
35
764-5
74
0167
0.972
0.000234
O.OI3I
00138
40
762.0
74
147
0.957
0.000232
0.0129
0.0139
45
761.7
74-
294
0.947
0.000229
0.0127
0.0140
50
760.9
74-
461
0920
0.000223
0.0124
0.0140
For q and also af>sofption coefficient, see Ethane, p. 285.
HEPTANK n CHi(CHs)fCH..
F.-pt. lowering data for mixtures of heptane and phenol are given by (Campett
and Delgrosso, 1913).
HEPTOIC ACm CH.(CHt)»COOH.
100 gms. HiO dissolve 0.241 gm. heptoic acid at 15^ (Lumsdeii, 1905.)
HKXAMK'itiYiJSNE (Hexahydrobenzene). See Cyclohexane, p. 280.
EEXAMETHTLSNB TETRAMINE (CH>)«N4.
100 gms. HsO dissolve 81.32 gms. (CHt)6N4 at 12^ (Ddepine, zSgsO
100 gms. abs. alcohol dissolve 3.22 gms. (CHt)6N4 at 12^ "
100 cc. 90% alcohol dissolve 12.5 gms. (CHt)6N4 at 15-20^. (Squire and Calnes, 1905.)
100 gms. CHCU dissolve 8.09 gms. (CHi)«N4 at 12 . pekpine, 1895.)
CeHii.
Solubility in Methyl Alcohol.
(Rothmund, 1898.)
Determined by synthetic method, see p. 16.
Gms. Hexane per 100 Gms. Gms* Hexane per xoo Gms.
^■"."^^""■^^^■^"^.■•^^"■^.^"^^
Alcoholic Hexane
Layer. Layer.
43-6 91-2
52.7 85.5
42.6 (crit. t.) 68.9
F.-pt. data for hexane + phenol. (Campetti and Delgroaao, 19x3.)
HZPPUBIG ACID aH»CO.NH.CHiCOOH.
Solubility in Several Solvents.
r.
Alcoholic
Hexane
r.
Layer.
Layer.
10
26. s
96.8
3S
20
31.6
95-9
40
30
38.3
93-7
42
SohrenL
f.
Gms.
r4H,C0.NHCH,C(X>H
per zoo Gms. Solvent.
Anthority.
Water
20-25
0.42
(Defan, 1917.)
Methyl Alcohol
22
9.80
(Timofeiew, 1894^
Ethyl Alcohol
22
5.20
M
Propyl Alcohol
23
2.80
«
50% Aqueous Pyridine
20-25
88
(Ddm, Z9Z70
311 HXPPUBIC ACID
Solubility of Hippuric Acid at 25** in Aqueous Solutions of:
Formic Acid. (EeodaU, 19x1.) Sodium Hippurate. (Sid^wick, 19x0.)
Nonnality Gms. Hippuric
of Aq. Acid per
HCOOQ. Liter.
Normality Gms. Hippuric
of Aq. Add per
HCOOH. Liter.
Normality of Gms. Hippuric
Aq. Sodium Acid per
Hippurate. Liter.
0
3 67
5
4.08
0
6.99(?)
I-2S
3 -61
10
4-77
I
i3-97(?)
2-5
372
mPPUBIO ACID CeH,CONH.CH,COOH.
Solubility in Aq. Potassium Hippurate Solutions at ao*.
(Hoitsema — Z. phyak. Chem. aTt 3X7t 'gS*)
Grams per Liter Solutioa.
002
008
X)eiisity Gram Mols. per liter Sol.
ofSolutioiis. C^gNOs. kCvHsNOs.
0.0182 O
0.0163 O.OII
0.0183 0.071
022 0.0234 0.254
114 0.064 1.36
182 O.I3I 2.21
192 0.147 2.32
19s O.IS3 2.40
201 0.133 2.50
239 0.084 3.01
282 0.068 3.57
282 0.065 3.58
276 0.031 3.56
277 O.OII 3.55
277 0.00 3.56
CANOs. KCftUsNOs.
3 276
2.919
3.278
4. 191
11.47
23.46
26.32
27.40
23.82
15.04
12.18
11.60
SS5
1. 917
o
2
IS
55
295
480
504
521
543
654
775
777
773
771
773
o
39
43
18
4
I
SoUd
Phase.
CbH»NQ»
I )CiH^C^+
^ \ Cgl^NOiXCANOaJbO
CANOaJLCANO^JiaO
4
I
o
7
8
4
3
4
1
CANOk.lCCVH^O».^0
+KCANOa
' KCANOi
HOLOCAINX H7DB0CHL0BIDE.
100 gms. HsO dissolve 2 gms. holocaine hydrochloride at 15-20^
(Squire and Calnes, z9qs.|
HOMATBOPINE H7DB0BR0MIDE Ci6H>iN0s.HBr.
Solubility in Water, etc.
(u. s. p. vm.)
100 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^
HTDBASTINE CuHnNOe.
CuHuNO^HCl.
Solubility in Several Solvents.
(U. S. p. Vni; at i8'-aa*, MQUer, 1903.)
HYDBASTININE HYDROCHLOBIDB
Gms. CnHi
Sdvent.
Water
Alcohol
Benzene
Ethyl Acetate
Petroleum Ether 0.073
flNO^pei
Solution.
per zoo Gms.
Sohrent.
Gms. per loo Gms. Solution
at i8'-2a'.
At i8»-2a». At 8o'. CnHjiN(V^CuHuNO|.Ha.
0.033 0.025 Ether 0.51 0.078(25"*)
0.74(25"*) 5.9(60**) Ether+HjO 0.80
8.89 ... Chloroform 100+ 0.35 (25^)
405 ... ecu 0.123
B7DBAZIDE8 an
H7DRAZIDES.
Solubility of thb Tautomeric Forms of Htdrazidbs in Benzene at 5^
Determined by the freezing-point method. See alao p. 4S7. (Sidgwkkp 19x5.)
Gms. Compound
Compound. Fonnula. Dissolved per
Liter Benzene.
SS
• CO V ) A form
Phthalylphenylhydrazide CjHi ^ ^^ > N.NH.CiHb J ^,
^ CO ^ ) C form
Z.I
/C0\
Phthalylphenyhnethylhydraade CA \ p^ / N J^(CHi)CA, A form 124
H7DRAZINE NH1.NH,.
Distribution of Hydrazine between Water and Benzene.
(GeoxgievicB, 19x5.)
Gmg. NHt.NH| per: Gms. NH.NHt per:
95 cc. H|0 Layer. 75 oc. C«H« Layer. 35 oc. H^ Layer. 75 cc. C«H« Layer.
0.4137 0.027 1. 7601 0.0626
0.6676 0.033s 2.3336 O.IIOI
1.0862 0.03SS 4-7S 0-137
HYDRAZINE PerCHLOBATE N,H4(HC10«)i.3HiO.
Solubility in Water. (Carlson, 1910.)
X. Sp. Gr. Gms. NsH4(HC104)«
* * Sat. SoL per zoo cc. Sat. SoL
18 1.264 41*72
35 I -391 66-9
HYDRAZINE MonoNITaATE N>H4.HN0,.
Solubility in Water. (Sommer, 1914-)
^ Gms. NtH^HNQi per 100 Gms. Gms. NtH4.HN0i per xoo Gms.
Sat. Sol. Water. Sat. Sol. Water.
10 63.63 174-9 40.02 85.86 607.2
IS 68.47 217.2 4502 88.06 737.6
20.01 72.70 266.3 50.01 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
H7DRAZINE SULFATE N,H4.HsS0«.
100 grams water dissolve 3.055 gms. NsH4.HsS04 at 22^ (Cuitius and Jay, 1889.)
Phenyl HYDRAZINE and other substituted hydrazines. See page 486.
HYDBIODIC ACID HI.
Solubility in Water, Determined • by Freezing-point Method.
(Pickering, x893a.)
Gm. HI
t*. per xoo Gms. Solid Phase.
Sat. Sol.
Ico
— 10
20.3
—20
293
-30
3SI
-40
39
-so
42
-60
44-4
-70
46.2
-80
47-9
M
M
««
Gms. HI
r.
per xoo Gms. Solid Phase.
Sat. SoL
-60
52.6 HI.4H/>
-40
59
about— 35.5 m. pt.
64
-40
65-5 -
-49
66.3 " +HI.3HdO
—48 m. pt.
70.3 HI.3Hd0
-S6
73.5 "+HI.aH/)
-52
74 HI 2H,0
" +HI.4IW)
F.-pt. data for HI + HiS (BagSter, 1911}, HI + (CHt)iO. (Maass and Mcintosh, Z9za.)
313
H7DR0BB0MIG ACID
HTDBOBBOMIO ACID HBr.
Solubility in Water.
(Rooaeboom— Z. phyrik. Chem. at 454f '88; Rec. trav. cfaim. 4« roj, 'Ss\ 5* S58» "Sd; aee also PIdcerintf
— PhU. Mag. is] 36» iig. ^JSO
Gms. mrDisolved at
Lower Ptcssuks per loo
Gms. HsO.
175.0 (10 mm.)
GmsSBr DianbedUt 760-7650110 j
t:
per 100 Gms.
fi.
Water.
Soludoa.
— a.
5 255.0
71 83
. • .
-IS
239.0
70.50
■ • •
0
221.2
68.85
611. 6
+10
210.3
67.76
581.4
IS
204.0
67.10
...
as
193.0
65.88
533 I
SO
171 S
63.16
468.6
7S
150.5
60.08
406.7
100
130. 0
S^'S^
344.6
108.5 (5 mm.)
• • •
• • e
For fi aee ethane, p. 285«
F.-pt. data for HBr + H,S (Bagster, 1911); HBr + (CHi)A HBr + CHiOH,
HBr + CtH,OH, HBr + CH,COOC,H« and HBr + CeH,CH,.
(Maaas and Mcintosh, 19x9.) (Rod and Mclntoah, Z9z60
H7DROCHLOBIC ACID HCl.
Solubility in Water by the Freezing-point Method.
(Composite curve from results of Roloff, 1895; Pickering, i893(a}; Roozeboom,
1884, 1889 and Rupert, 1909.)
f.
— 1.706
-14.97
-28.84
-40
-60.
-80
-86Eutec.
-50
-40
-30
— 24.9 m. pL
-27.5
-23.8
— 21.2
Gin8.Ha
per xoo Gms.
Sat. Sol.
1.66
10.02
14 SI
17.40
21.30
24.20
24.8
30.1
32.7
36.5
40.3
44
45.7
45.9
SoUd Phase.
Ice
r.
M
M
U
««
+Ha.3H|Q
Ha.3H^
«i
•• +HaaIW)
HaaH^
— 18.4 48.6
— i7.7m.pt. 50.3
-18.7 52.85
-19.4 54.1
-20.8 55.7
-21.3 56.5
-23.2 57.3
— 23.5Eutec. ...
-21.5 58.2
— 20.7 59.1
— 18.4 61. 1
— 17.4 62.4
-15.4 65.4
-15.35 66.8
Gms. Ha
per xoo Gms. Solid Phase.
Sat. Sol.
HaaH^
M
" +Hajaio
Ha.H^
At about — 15.35 two liquid layers are formed. Data for these are as follows:
HCl layer. HiO layer.
/ * N / ■■ ■ A I — _ ■%
M^ Gms. ILO Gms. HQ Gms. HD
Satuxi^on per xoo Gms. t*. per xoo Gms. tf. of Sat. Sd. t*. per xoo j3,ms. i. of Sat. SoL
'^ Sat. 501.
Below —50
" -SO
Bet. — isando*
Above 45
it
tt
Sat. Sd.
0.008
0.017
0.077
0.02Z
0.052
O.II
0.13
—20
-15
— 10
-s
o
+s
ID
67.6s
67.29
66.71
66.44
6S.8S
65.48
65.18
1.279
1.269
Z.260
I.2SS
1.247
I.24S
1.240
IS
20
30
35
40
4S
SO
Sat. Sol.
64.70
64.19
63.21
62.90
62.27
61.76
61.65
X.231
Z.228
Z.229
Z.227
Z.218
X.2I2
Z.2Z9
For additional data on this system see Baume and Tykociner, 1914.
H7DB0GHL0BZG AGID
314
HTDBOOHLOBIO ACID HCl.
Solubility in Water at Dippbrbnt Tbmpbraturbs and
Prbssurbs.
(Ddcke; Ronoe and Dittmar — liebig's Ann. i ia« 334* *59; hdam o*. Rooaebooift — Rec. tntT.
chim. 3» 104,^84.)
At Different Temperktures and 760 mm.
Ptbhiik.
At Different Pressures fnd e*
»••
ocHClper
loooc.HiO.
Deoatj.
Cms. Ha per
loeg. SoL
Gma.Haper
xoo g. HsO.
Presauret.*
Gma.Haper
loog. HiO
0
525 a
t.22S7
45 IS
82.31
60
61.3
4
497 7
1.3265
44 36
79 73
100
65-7
8
4803
1.2185
4383
78.03
150
68.6
13
471 -3
1.2148
43 28
76.30
200
70.7
14
463 4
1.2074
42.83
74.92
300
73-8
18
4S»-2
X.2064
43 34
73-41
400
76 -3
23
4350
I. 2014
41 54
71 03
500
78.3
30
• • •
■ •
40.23
67 -3
600
80 -o
40
• • •
• • •
38.68
63 -3
750
83.4
so
• • •
• • •
37-34
59-6
1000
85.6
60
• • •
• • •
35-94
56.1
1300
895
^ PffBasuiM ill mm. Hg minus tenaioa of HaO vapor.
Solubility in Water at Tbmperaturbs Below o*.
At a pressure of 760 mm.
f.
«•
r.
9-
24
IOI.2
-IS
93.3
21
98.3
— 10
89.8
18.3
96
- S
86.8
18
95.7
0
84.2
At pressures below and above 760 mm.
t*. mm. Pressure. 9.
— 23.8
-21 334
-19 580
— 18 900
-17.7 1073
For definition of q, see Ethane, p. 285.
ror dennition ot q, see fLtnane, p. 205.
The eutectic is at —86^ and 33 gma. HCl per 100 gma. HgO.
84.2
86.8
92.6
98.4
101.4
Solubility op Hydrochloric Acid Gas in Mbthyl Alcohol, Ethyl
Alcohol, and in Ether at 760 mm. Pressure.
CAo BruTA— Rec. tour. chin. xi« tag* *9»l Schuncke — Z. piiyak. Chenu Z4« 3361 'mO
Grains HCl gas per xoo Grams Solution tn:
» .
dHaOH.
CiBiOH.
(CiH,)iO.
— 10
(4. 6
• • •
37. SI (-9a')
- 5
• • •
• • a
37-0
0 .
s^ 3
45-4
35 6
+ S
...
44.2 (6.5")
33 I
10
• • •
42.7 (II. s°)
30 3S
IS
• . .
• • •
37.62
20
47.0(18'')
41.0
24.9
«s
• • •
40.3 (23. s**)
22.18
30
43 •0(31-7*')
38.1 (32°)
19.47
315
H7DB0GHL0BIG AGZD
Solubility op Hydrochlokic Acid Gas in Aq. Sulfumc Acid Solutions.
(Coppadoro, 1909.)
i of Sat.
SoL
Results at I7^
Gms. per xoo Gms.
Sat. Sol.
K«S04.
I
I
I
I
I
I
I
I
I
I
I
I
I
211
220
220
260
305
3SS
430
S4S
580
660
735
81S
o
1.86
4.7s
8.04
12.80
20.9
30.8
44.6
59-4
65.4
73.7
77. S
89
HCl.
42.7
39-9
39-2
36.9
33-2
28.5
22.6
IS
6.26
3-25
0.62
O.II
0.068
iof Sat.
SoL
1.18s
I 195
1. 210
I.2SS
1. 255
1.340
1.400
1.520
I.S7S
1.650
I 725
I -755
1.770
Results at 40^
Gms. per xoo Gms.
t. Sol.
HtSO«.
3.56
5.86
8.90
16.80
18.8
28.6
44.2
61. 1
66.4
73-2
79-4
81.4
83.5
HQ. •
35-6
34.8
32.4
27.6
25-9
18.5
"5
3-3S
1. 17
0.17
0.081
0.032
0.029
i of Sat.
SoL
I.I4S
1. 150
1. 160
1. 180
1.225
1.230
1-313
1.380
1. 510
1.560
1.700
1-745
1. 745
Results at 70^
Gms. Dcr xoo Gms.
Sat. Sot.
H|SO«.
1. 61
3-38
4.80
7-93
18.9
20
36.2
48
62.7
67.6
80.7
83
83-4
HQ.
32.7
3I-I
30.5
28.9
22.8
22.3
13-2
6.99
1.56
0.54
0.05
0.035
0.032
MisciBiLiTT OF Hydrochloric Acid with Mixtures of Watbr and
Phenol at 12°.
(SchrememakexB and van der Horn van der Bos, 19x2.)
Compodtion of the Reciprocally
Saturated Liquid Pairs.
Composition of the Solutions in
Contact with Solid Phenol.
Water Rich Layer.
% HO. % Phenol.
Phenol Rich Layer.
% HQ. % Phenof.
% Water.
K
%Ha.
%PhenoL
0 7.45
0 72
11.22
0
88.78
3.1 6.6
0.09 78
84.5
10.7
4.8
6.6 5-3
0.2 80.3
80.38
15-64
3-98
8 5.1
0.36 82.6
72.43
24.37
3-2
10.7 4.8
0.52 84.5
60.25
36.25
35
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 Add + Hydrogen Sulfide (Baume and Geoigitaes. 19x2, x9X4)
4- Mpthvl Alrnhni / (Baume and Borowaki, 1914; Baume and PamlQ,
-t- JVietnyi Aiconol ( ,g„ ,g,^. ^^^^ and Mcintosh, 19x3.)
+ Methyl Chloride (Baume and Tykodner, 19x4.)
+ Methyl Ether (Maass and Mclntoah, 19x3; Baume, X91X, 1914.)
+ Propionic Acid (Baume and (jeoigitses, 19x2, X9X4.)
+ Sulfur Dioxide (Baume and Pamfil, x9xxp 19x4)
41
it
II
II
II
H7DBOCTANIC ACID HCN.
Distribution between Water and Benzene.
(Hantach and Sebalt, 1899; Hantiwch and Vagt, 1901 .)
Mol. HCN per Liter:
r.
6
16
25
Mol. HCN per Liter;
B^ Layer (c). CA Layer (<;')•
0.00625 0.00325 I
923
r.
7
20
B,0 Layer (c). C|H| Layer (O*
0.0574 0.0148
0.0572 0.0154
7
0.00593 0.00363 1.634
0.00580 0.00375 1.547
Data for the effect of HCl and of KCl on the distribution are also given.
3.88
H7DB0FLU0BIC ACID HF.
100 grams HiO dissolve iii grams HF at ~35^
(Mctawr, Z894O
BYDBOQIN
316
BTDBOOEH H.
Solubility in Water.
(Winkkr — Ber. a4t 99i '91; Bohr and Bock — Wied. Ann. 44* 3x8» '9X1 Ttmoi^lew— Z. phydc
Cbem. 6, 147* '90.)
r.
I.
^.
0
0.0214
^
• • •
• • •
00214
0.000193
s
0.0203
0
.0209 —
0.0241
0.0204
0.000184
10
0.0193
0
.0204 —
0.0229
0.0195
0.000176
IS
0.0185
0
.0200 —
0.0217
0.0188
0.000169
so
0.0178
0
.0196 —
0.0205
0.0182
0.000162
«S
0.0171
0
.0193 -
0.0191
0.017s
0.000156
30
0.0163
0.0170
0.000147
40
00153
0.0164
0.000139
SO
0.0141
0.0161
0. 000x29
60
0.0129
0.0160
0. 0001 19
80
0.0085
0.0160
0.000079
100
0.0000
•
0.0160
0.000000
\ , A mmmn
Id Solubility
^ Expression,
see p. 227.
Fori9', B, and
0. see Ethan
Data for the solubility of hydrogen in water at pressures up to 10 atmospheres
are given by Cassuto, 1913.
BOLUBILITY OF HYDROGEN IN AqUBOUS SOLUTIONS OP AciDS AND
Bases at 25^
(Gc£fcken— Z. phyiik. Chem. 49, 968, '04.)
(jTunEoniT.
Adds and
SoluUUty of H (is - OstwaJd Expression) in Sohidoos of:
per liter. ^^'
0.0 0.0193
0.5 0.0186
i.o 0.0179
8.0 0.0168
3.0 0.0159
4*o • • •
HNO|. iHaS04. CHgCOOH. CHsQCOOH. KOH. NaOH.
0.0193 0.0193 0.0193
0.0188 0.0185 0.0192
0.0183 0.0177 O.OI9I
0.0174 0.0163 0.0188
0.0167 0.0150 0.0186
0.0160 O.OI4I 0.0186
0.0193 0.0193
0.0189 0.0167
0.0186 0.0142
0.0180
0.0193
0.0165
0.0139
0.0097
0.0072
0.005s
The above figures for the conoentratiom of acids and bades were calculated to
grams per liter, and these values with the corresponding lu values for the solubility
of hydrogen, plotted on crosa-section paper. From the resulting curves, the follow-
ing table was read:
Grams Adds
SolubiHty i
3fH(l26-C
>Btwa]dEzpi
«a8ion)inSo]
ludons of:
per litrr. HQ.
HNOs.
iHsSO«. CHsCOOH.
CHsQCOOH
:. KOH.
NaOH.
0 0.0193
00193
0.0193
0.0193
0.0193
0.0193
0.0193
30 0.0185
0.0189
o.oi86
0.0192
O.OI9I
0.0172
0.0165
40 0.0x79
0.0186
0.0180
O.OI9I
0.0190
00153
0.0140
60 0.0173
0.0183
0.0174
0.0190
0.0188
0.0135
O.OII7
80 0.0167
0.0180
0.0168
0.0189
0.0187
0.0097
100 0.0160
0.0179
0.0162
0.0189
0.0185
0.0082
150
O.OI71
0.0148
0.0188
0.0182
0.0058
200
0.0165
0.0140
0.0186
0.0179
• • •
250
0.0160
■ • ■
00184
• • •
• • •
For Ostwald Solubility Expression /, see p. 227.
The Solubility of Hydrogen in Conc. HtSOi at 20*.
(Christo£f, 1906.)
%H2S04 o 35.82 61.62 95.6
In 0.0208 0.00954 0.00708 0.01097
317
HTDROCm
Solubility op Hydrogen in Aqueous Solutions op Ammonium
Nitrate at ao**.
(Knopp— Z. phyaQc. Chem. 48. 103, Vh*)
0.00
I 037
2.167
3 378
4.823
6.773
11.550
Normafity
(per xooo GmsO
HiO.
0.00
0.1308
0.2765
0.4363
06333
0.9069
1.6308
Mokcnkr
ConoentiBf*
tion.
0.00
0.002352
0.004956
0.007799
0011280
0.016447
0.028525
Abflorpdan
Coefficient
of Hydrofdia
0.0188
o. 01872
0.01845
0.01823
0.01773
o. 01744
0.01647
Density
of SolutioQa.
1.0027
1.0072
I. 0122
1 .0182
1 .0262
1.04652
80LUBILITY OF Hydrogen in Aqueous Solutions of Barium
Chloride.
(Bnim— Z. phyiik. Chem. 33, 735t 'ooO
Coefficient of Abeoiption of Hydrogen at !
GBH.BaClt
per xoo Gmi.
Solntiop.
0.00
3.29
3.6
6.45
7.00
5*.
0.0237
0.02II
0.0209
0.0196
0.0194
io».
0.0221
0.0198
0.0197
00186
0.0183
IS**.
0.0206
0.9185
0.0184
0.0173
0.0172
90».
O.OI9I
0.0172
0.0170
00161
0.0159
•5*.
0.017s
00157
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. z8» 14, '95O
Coefficient of Absorption of hydrogen in water at 15^ - 0.01883.
In Calcitun In Magnesium In Lithitim
Stdphate.
Chloride.
Gma. G. M.
CaCls CaOa
100 g. Sol. iSet.
3.47 0.321
Chloride.
Abeoiption
Coefficient
of H.
Gms. G>M. Aw»wn*<,«—
MgSO. MgSO, ^5S£5
per per
100 g. Sol. Liter.
Coefficient
of H.
6.10
"33
17.5a
a6.34
0.578
1. 122
0.01619
0.01450
o. 01 138
X.1827 0.00839
2.962 0.00519
4-97 0-433 0.01501
10.19 0.936 o. 01 159
23.76 2.501 0.00499
Gms. G. M. *i,-j^,j»,^
LiCl Lia ^^^
ioog!sol. iSSt. ^^'
3.48 0.835 O.O1619
7.34 1.800 0.01370
M.63 3.734 0.0099
For definition of Coefficient of Absorption, see page 227.
Solubility of Hydrogen in Aqueous Solutions
Carbonate, Chloride, and Nitrate at
(Gordon.)
In Potassium
Carbonate.
Gms.
K«CQ»
per
too g. Sol.
In Potassitim
Chloride.
In
OP Potassium
15^
Potassium
Nitrate.
2.82
8.83
16.47
24.13
41.81
G.M.
K^Oft
per
liter.
0.309
0.690
1.376
2.156
4.35a
Abeorption
Coefficient
of H.
Absorption
Coefficient
of H.
0.01628
O.OI183
0.00761
0.00462
0.00160
Gms. G. M.
KQ KCl
per per
100 g. Sd. Later.
3.83 0.526 0.01667
7.48 1. 051 0.01489
12.13 1-755 0.01279
19.21 2.909 0.01012
22.92 3.554 0.00892
Gms.
KNOft
per
100 g. Sol.
4.73
8.44
16.59
21.46
G. M. «•_ ..
^^ oS^e
Dter. *^^-
0.482 0.01683
0.879 0.01559
1.820 O.OI311
2.430 o.oxx8o
HYDBOQBf
318
Solubility of Hydrogen in Aqueous Solutions of PoTASsixm
Chloride and Nitrate at 20®.
(KAopp— Z. plqrrik. Chem. 48, 103, '04.)
1.089
2.123
4.070
6.375
7 380
23. 6X2
In Potassiiun Chloride.
Normality
(per 1000
g.H,0).
O.I47S
Abionytion
Cocfficie&t.
0.2907
0.5687
0.9127
1.0683
a. 1222
0.01823
o. 01757
O.OI66I
O.OI53I
0.01472
O.OI2SS
of
Solutiaat.
I 0052
I.OI18
1 .0243
1 .0394
1.0460
1.087s
In Potassium Nitrate.
Aburpdoo
Normality
p, (per 1000
C HsO).
1.224 0.1245
2.094 O.2II4
4.010 0.4127
5.925 06225
7.742 0.8293
13-510 1.5436
0.01835
O.OI818
0.01785
0.01743
0.01667
O.OZ436
of
Solutiooa.
1.0059
1 .0113
1 .0236
I 0359
I 0477
i.o86j
Solubility of Hydrogen in Aqueous Sopiuu Carbonate
Sulphate Solutions at 15^.
((j«rdoo.)
AND
In Sodium Carbonate.
Ni
per 100
Solntioifc.
«I5
8.64
"S3
CM.
NagCOi
per liter.
0.207
0.438
1.2X8
Abaorption
ofH.
0.01639
0.01385
0.00839
In Sodium Sulphate.
Gma. Naj^4 G. M. Abaorpllaa
per 100 urns. NaaSQ« CodbataX
Sdutioo. per Liter. of H.
4-5^ 0.335 0.01519
8.42 0.638 0.0154
16.69 1-364 0.00775
Solubility op Hydrogen in Aqueous Solutions of Sodium
Chloride.
(Bnun; (}ordoa.)
(}mi.NaCI
per xoeGma.
Solutkn
1-25
3&>
4.48
6.00
14.78
23.84
Coefficient of Abaorptioo of Hydrogen at:
0.0218
0.0198
0.0192
0.0184
xo».
0.0205
0.0188
0.0x83
0.0175
15'.
0.0I9I
0.0176
0.0I7I
0.0164
0.0093
0.00595
ao'.
0.0177
0.0162
0.0159
0.0153
0.0162
0.0148
0.0143
0.0138
Solubility of Hydrogen in Aqueous Solutions op Sodium
Nitrate.
In Soditmi Nitrate at 20^
(Knopp.)
I.04X
2.192
4.405
6.702
12.637
In Soditmi Nitrate at 15^
(Gordon.)
Normalitjr
(per 1000
Gms. H«0).
0.1236
o . 2634
05416
0.8442
1-7354
Abaorpdon
Coefficient
OfH.
0.01839
0.01774
0.01694
O.OI518
0.0130
Denaitr
of
Solutions.
I
I
I
Z
I
0052
0130
0282
O44II
08667
Gm8.NaNOt
per 100 Gma.
Solution.
5-57
II. 16
19.77
37.43
G.M.
NaNQs
per Liter.
0.679
1-413
2.656
5-7"
Abiorptioii
CoeffidenI
OfH.
0.01603
0.0137
0.01052
0.00578
319
HYDROOEN
Solubility of Hydrogen in Aqueous Solutions of Various Salts at 15^.
(Stdner. 1894.)
Salt in Aq.
Solution.
LiCl
KNQi
iAlClt
KCl
NaNOi
iCaCli
NaCl
iMgS04
iZnS04
iNaiSO*
iKtCQi
iNatCQ,
Cane Sugar
Bunien Abaorptfam Coefficient fi (XioO >» Aq. Solution of Normality.
o.
1883
1883
1883
1883
1883
1883
1883
1883
1883
1883
1883
1883
1883
X.
574-
524
S"
502
496
493
478
4SI
446
370
338
340
280
a.
1325
1276
I22I
I217
1 201
"95
II44
II20
III3
991
967
699
3-
II2I
1076
993
996
984
958
880
856
852
710
700
4-
949
• * •
810
820
808
780
699
659
667
6.
667 sso
667
63s
573
499
510
542
510
508 372 273 206 158
731
Solubility of Hydrogen in Alcohol. (Timofdew, 1890; Bunsen-Heorich
Coef . of Absorp-
.8% V,
r.
tion in 98.8 yo
' Alcohol.
Coef. of Absorp-
tion in 7%
Alcohol.
f.
189a.)
iTDtic
xuiol
o 0.0676 4 0.0749 I
6.2 0.0693 18.8 0.0740 s
.13.4 0.0705 II. 4
23-7
Solubility in Aqueous Alcohol Solutions at 20^ and 760 mm. Pressure.
(Lubanchp 1889.)
Coef. of Absoi
in Puxe Alcol
(Bunaen).
0.06916
0.06847
0.06765
0.06633
ion
Vol. % Absorbed H.
1-93
1-43
1.29
1. 17
Solubility of Hydrogen in Aq. Solutions of Chloral Hydrate.
(MOller, C. Z9xa-Z3.)
Absorption Coefficient.
d^ of Aq. i ^ \
Solution.
Wt. % Alcdkd.
O
9.09
16.67
23.08
Wt. % Alcohol.
28.57
33-33
so
66.67
Vol. % Absorbed H.
1.04
1. 17
2.02
2.5s
r.
Cms. Chloral
Hydrate per
100 Cms. Aq.
Sol.
19.4
17.4
18.7
16.5
17
17.9
18.3
iS-5
28.3
46.56
52
63
68
78.4
1 .0722
1. 143
I • 2505
I . 2870
I 371
1.4097
1-4993
0.01732
0.01569
0.01388
0.01314
0.01270
0.01286
0.01398
0.01724
0,01540
0.01375
0.01280
0.01243
0.01270
0.01380
Solubility of Hydrogen in Chloral Hydrate Solutions at 20^ (Knopp, 1904.)
Normality (per
zoooGms. HflO).
0.310
0.504
1.030
2-530
3 770
6
10.700
4.91
7.69
14.56
29.50
38.42
49-79
63.90
For definition of Bunsen Absorption Coef., see p. 227.
Molecular
Concentration.
0.005594
0.008992
0.018223
0.043601
0.063647
0.097493
O.161660
Absorption
Coefficient of H.
0.01839
0.01802
O.OI712
0.01542
0.01440
0.01353
0.01307
Density
of Solutions.
1.0202
1.0320
1.0669
I . 1466
I . 1982
1.2724
1-3743
HTDBOaXN
330
Solubility of Hydrogen in Aqueous Solutions of Glycerol.
Results at 14^ and 21**. (Henkd, 1905. 191 3.) Results at 25^ (Dnicker and Molet, 1910.)
14
u
ii
ii
u
it
31
u
It
it
it
u
Wt. %
Glycerol.
O
2.29
S-32
8.57
10.83
15-31
O
2.29
S.68
6.46
10.40
18.20
Absorp. Coef.
0 (See p. aa?.)
0.0193
0.0189
0.0186
0.0182
O.O1815
0.01765
0.0184
O.OI81
0.0177
0.0176
O.QI7I
0.0160
Wt. %
Glycerol.
O
4
los
22
49.8
50.5
52.6
67
80
88
95
^U Sat. Sol.
I
I.OIOI
1.0260
1.0542
I. 1290
I. 1300
I • 1365
I. 1752
I.2II3
I. 2159
I . 2307
I . 2502
In (Ofltwald
Expression).
0.0196
0.0186
0.0178
0.0154
0.0099
0.0097
0.0090
0.0067
0.0051
0.0051
0.0044
0.0034
Additional data for this system are given by MQller, C. 1912-13.
Solubility of Hydrogen in Aqueous Solutions op Several Compounds.
(HOfner, 1906-07.)
Aqueoui Solution of:
Water alone
Dextrose (Grape Sugar)
It
tt
Urea
Acetamide
Alanine
Glycocol
Cone, of
Solvent Gnu.
per Liter.
O
41.4s
87.3
174
60
S9
89
75
t. Absorption Coef. fi,
20.11 O.O181
20 0.0176
20.25 0.0166
20.28 0.0152
20.17 0.0170
20.11 0.0180
20.08 0.0156
20.16 0.0158
S(».UBiLrrY OP Hydrogen in Aqueous Solutions of Cane Sugar and
OF Grape Sugar. (Moiier, c. 19x3-13)
f.
iS-2
II. 6
12
12.7
II. 8
133
12.6
Wt. %
Cane
Sugar.
5 04
14.7
20.26
29.86
31 -74
39.65
42.94
Sp. Gr.
Sat. Sol.
Abs. Coef.
fin-
dii
du
du
d\%
= 1.019 0.0173
= 1.060 O.OI5I
= 1.084 0.0146
= 1.128 0.0126
= 1.138 O.OII9
rfw.6=i.i7S 0.0103
^12.5 =1.195 0.0094
193
20.5
20.5
21. 1
21.8
21.2
Wt. %
Grape
Svigar.
O
Sp. Gr.
Sat. Sol.
Abs. Coef.
fin-
0.0184
0.0160
O.OI4S
12.2 ^10=1.048
20.7 (^=1.084
32.56 (^=1.130 0.0125
45-8 (^=1^.199 0.0102
59 (^=1.266 0.0078
Solubility of Hydrogen in Aqueous Sugar Solutions at 15*. (Gordon. 1895-)
Gnu. Sugar per Gm. Mob. Sugar Absorption
100 Gms. Solution. per Liter. Coefficient of H.
16.67 0.520 O.OI561
30.08 0.993 0.01284
47.65 1.699 0.00892
Solubility of Hydrogen at 25** (Findlay and Shen, 1912) in Aq. Solutions of:
Gelatin.
Gms. Gdatin 1
per ioo cc. **
1.53 0.0194
2.69 0.0189
4.74 0.0185
5.71 0.0182
Gms. Dextrin
perxoooc.
3 98
8.58
8.12
19.20
»trin.
Starch,
Sp. Gr.
J..
Gms. Starch
per xoo cc.
Sp. Gr.
In-
1. 012
0.0194
2.01
1. 005
0.0194
1. 019
O.OI91
3.56
I. Oil
0.0189
1.028
0.0188
7.13
1.024
O.O181
1.066
0.0174
9.29
1.032
0.0182
321
HTDBOaXN
SOLUBILITT OF HYDROGEN IN AqUBOUS PROPIONIC AciD SOLUTIONS.
(Bnum, X900.)
Cms. C|H|CXX)H
per zoo Gms.
Solution.
Caeffident of AbsoipCkn of Hydzogen at:
A
5*.
lO*.
IS*.
ao*.
as*.
2.63
0
.02245
0.0214
0.0200
0.0188
0.0172
3-37
0
.0222
0.0212
0.0199
0.0187
O.OI7I
S-27
0
.0224
0.0212
0.0198
0.0184
O.OI7I
6.50
0
.0218
0.0209
0.0193
0.0183
0.0169
9.91
0
.0213
0.0203
O.OI9I
0.0178
0.0160
SOLUBILITT OF HYDROGEN IN RUSSIAN PETROLEUM.
(Gniewass and Walfiss, 1887.)
G)effident of absorption (see p. 227) at 30^ « 0.0582, at 10^ *>■ 0.0652.
Solubility of
Results in terms of
SohrtniL
Water o.
Aniline o.
Amyl Alcohol o.
Nitrobenzene o.
Carbon Disulfide o.
Acetic Add o.
Benzene o.
Acetone o.
Hydr
OGEN IN y
IVater and in Organic
S(X.VENTS.
the Ostwald Expression, see p. 227.
awt. X90X.)
Im.
^.
Solvent.
Im. ^
0199
0.0200
Amy] Acetate
0.0774 0.0743
0285
0.0303
Xylene
0.0819 0.0783
0301
0.0353
Ethyl AceUte
0.0852 0.0788
0371
0.03S3
Toluene
0.0874 0.0838
0375
0.0336
Ethyl Alcohol (98.8%)
0.0894 0.0862
0633
0.0617
Methyl Alcohol
0.0945 0.0902
0756
0.0707
Isobutyl Alcohol
0.0976 0.0929
0764
0.0703
Solubility of Hydrogen in Ethyl Ether.
(Christoff, Z9Z3.)
Results in terms of the Ostwald Solubility Expression / (see p. 227).
/o"0.iii5, /t « 0.1 150, /io = o.ii95, /li » 0.1259.
Data tor the solubility of hydrogen in metals are given by Sieverts and co-
workers* 1909, 1910, 1912.
HYDBOaKN PIBOZIDK HlQ^
Distribution of Hydrogen Peroxhw between Water and Amyl Alcohol
AT 0"
AND AT 25^
(Calvert,
1901;
Joyner, 19x2.)
Results at 0^ (Calvett, Joyner.)
Results at 25*". (Cahrert)
Mob.H,
^ per Liter.
-* V
Alcohol Layer {A).
W
A
Mob. ILf^t per Liter. m
k^ layer (IF).
H|0 Layer (IF).
Alcohol Layer (i4)^. ^
0.146
0.0216
6.76
0.094
0.013 7-<5i
0.200
0.030
6.66
0.194
0.028 6.91
0.407
0.061
6.63
0.297
0.042 7.08
0.749
O.II3
6.66
0.670
0.09s 709
1.970
0.293
6.71
0.913
0.130 7.01
Data are also given for the distribution of hydrogen peroxide between aqueous
sodium hydroxide solutions and amyl alcohol at o** ana at 25^
H7DBOOKN PEROZIDK
322
Distribution of Hydrogen Peroxide between Water and Organic Solvents.
(Walton and Lewis, 1916.)
DifiFerent amounts of perhydroi (30% HiOt solution) were added to various
mixtures of water and organic solvents and, after constant agitation for about
I hour, the HiOt in each layer was determined.
Ratio,
Solvent
Cone.
•q.
Solvent.
Cone. o«s. aolvcat
Ethyl AceUte
25
3.92- 4. II
Methyl Iodide
Isobutyl Alcohol
25
2.58- 2.63
m Toluidine
Amyl Acetate
25
13 -13 ■ 2
Phenol
Acetophenone
25
5.82- 6.06
Quinoline
Ether
25
8.28- 9. II
«
Ether
0
5.72- 5.85
u
Aniline
25
4.08- 4.10
r.
25
25
25
o
25
40
Ratio,
Cone. aq.
Cone. ofg. lolvau
Approz. 200
Approz. 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, 19 14.
Ratio, _ Ratio, Ratio,
Solvent. ^Q°<^- •<»•
Solvent.
Cone.
•q.
Solvent.
Cone.
•q.
Cone. ogg. tolTcnt Cone. oifi. lolvcBt Cone. otg. atArtat
Ethyl Acetate } Ethylisovalerianate ^ Isobutyl Alcohol |
Nitrobenzene ^ Isoamyl Propionate ^ Propyl Formate i
Acetophenone ^ Chloroform -^ Isobutyl Butyrate ^
Amyl Acetate i Benzene ^ 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.)
HTDBOaXN
SELENIDK H,Se
Solubility in Water.
(de Forerand and Fonze»-Diacon, 190a.)
t".
Vol. HsSe (at o^ and 760 mm.) dissolved
per I vol. HiO
3.77
9.65
3.45
13.2
3.31
22.5
2.70
HTDBOaXN SUUIDK H>S.
Solubility in Water.
(Winkler, 1906, 191 a.)
r.
Abs. Coef . 0.
q.
f.
Abs. Coef. ^.
q. t*. Aba-Coeff.^. q.
0
4.621
0.699
25
2.257
0.334 60
I. 176 0.146
5
3.935
0.593
30
2.014
0.295 70
1. 010 0.109
10
3 362
0.505
35
1. 811
0.262 80
0.906 0.076
15
2.913
0.436
40
1.642
0.233 90
0.835 0.041
20
2.554
0.380
SO
1.376
o.ii^ too
0.800 0
Solubility ]
[n Water and in Alcohol
, AT t^ AND 760 MM. PRESSURE.
(Bunsen and Carina; Fauser, x888.)
In Water.
In Alcohol.
i-.
I Vol.
H,0 Absorbs.
fi.
g. X Vol. Alcohol Absoibs.
0
4.37 Vols. H,S (at o*aiid 760]
nm.)
4.686 0
.710 17.89 Vols. H9S (at 0* and 760 mm.)
5
3.97
M
4.063 0
.615 14.78
M
10
3.59
II
3 520 0
.530 11.99
M
15
3.23
«
3.056 0
.458 9.54
«
20
2.91
M
2.672 0
.398 7.42
«
25
2.61
M
• ■ •
5.96(24^)
«
30
2.33
U
• • •
i • • • • •
35
2.08
U
• • •
i • • • • •
40
1.86
U
• • •
» • • • • •
For fi and q see Ethane, page 285.
The PT and the Px curves for the system HjS + HtO are given by Scheffer, 1911.
323
HYDBOGXN SULFIDB
S(X.UBILITT OF HyDROGBN SuLFIDB IN AqUBOUS SOLUTIONS OF HyDRIODIC
Acn> AT 25** AND 760 MM. TOTAL PRESSURE.
CPoQitzer, 1909.)
Mob. per Liter.
Gms. per Liter.
Mols. per Liter.
Gms. per Liter.
IH'J.
0.20
1.23
1.74
2.18
2.92
3-71
IHI].
o
1. 01
1. 51
1.93
2.64
3.42
0.1040
O.III
0.II3
0.125
0.138
0.142
HI.
O
129.2
193.2
246.9
337.8
437.5
HtS.
3-54
3.78
3.85
4.26
4.70
4.84
[HI. [HIJ. IHtS].
4.71 4.38 0.163
5.33 5.005 0.165
6.06 5.695 0.181
7.33 6.935 0.197
9.75 9.21 0.267
' HI.
H.S.
560.4
640.3
728.6
887.2
5. 55
5.62
6.17
6.71
"79
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 HsS and CHjOH and HtS and
(CH|)sO are given by Baume and Perrot, 191 1, 1914*
SOLUBILITT OF HYDROGEN SULFIDE IN AqUBOUS SaLT SOLUTIONS AT 25^
(McLauchlan, 1903.)
I
Note. — The original results are given in terms of j- which is the iodine titer (Q
of the HtS dissolved in the salt solution, divided by the titer (A>)» of the HtS 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 HtS absorbed by i vol. of aqueous solution.
Sdutioa.
Grams Salt
per Liter.
/ Vols. HtS
j^' per X Vol. Sol.
Solution. Gms^Sdt
1. Vo]ft.HtS
S periVoLSoL
wNHiBr
98
I
2.61
fiKBr 119
0.945
2.47
wNHiCl
53.4
0.96
2.40
nKCl 74.5
0.853
2.22
«NH«NO*
80
0.99
2.58
»KNOi loi
0.913
2.38
in(NH4)tS04
33
0.82
2.14
JnKtSO* 43.5
0.78
2.04
}n(NH4)tS04
16.5
0.91
2.37
inKtS04 21.7
0.89
2.32
wNH^CtHiO*
77.1
1.09
2.84
fiKT 166
0.98
2.56
n (NHt)jCO
60.1
1.02
2.66
n NaBr 103
0.93s
2.44
i»HCl
18.22
0.975
2.54
wNaCl 58.5
0.847
2.21
}nH,S04
24.52
0.905
2.36
} n NaCl 29 . 2
0.93
2.42
nCJWt
ISO
0.944
2.46
»NaNOi 85
0.893
2.32
3»C4H806
450
0.858
2.24
inNatS04 355
0.73
1.90
Pure C,H,(OH),
1000 •
0.863
2.26
inNa2S04 17.8
0.855
2.23
Similar data are also given for the solubility of HtS in aq. CtH«OH solutions
and in aq. CHsCOOH solutions at 25®.
HTDBOQUINOL (Hydroquinone) C6H4(OH)t 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^ (Aschu, zszj.)
HTDBOQUINOL 334
Solubility of Hydroquinol in Sulfur Dioxide in the Critical Vicinitt.
(Centnenwer and Teletow, 1903.)
Determinations made by the Synthetic Method, for which see Note, p. 16.
M Gns. HydroqiUBol ^ Gms. Hydroquinol m Cms. Hydroquinol
* * per 100 Gnu. SO^ * ' per 100 Gms. SO^ * * per zoo Gms. SO^
63 0.89 117. 6 4.46 136.7 10.31
73S 1-22 123.3 5-66 141.4 13.3
89.2 2.18 134-2 8.31 145 14.9
Distribution of Hydroquinol between Water and Ether at 15^.
(Pinnow, 191 x.)
Cone* Hydroquinol in: Cone. Hydroquinol in:
IV> Layer.
Father Layer.
H«0 Layer.
" \
Ether Layer.
0.00502
O.OIII
0.0502
0.127s
O.OII96
0.0249
0.0818
0.2343
0.0128
0.0274
O.IIO5
0.3543
0.0236
0.0552
O.1411
0.5300
0.04SS
O.II48
0.1502
0.5604
* The terms in which the oonc. is espressed axe not stated.
Freezing-point Data (Solubility, see footnote, p. i) are Given for the
Following Mixtures:
Hydroquinol and Naphthalene. (Kremann and Janetxky, xgza.)
" Pyrocatechol. (Jaeger. 1907.)
" " Resorcinol.
" " p Toluidine. (Philip and Smith, 1905.)
Monochlorohydroquinol and Monobromohydroquinol. (KOster, 1891.)
Diacetylmonochlorohydroquinol and Diacetylmonobromohydroquinol.
(Kllster, 191X.)
HTDBOXTLAMINE NH,(OH).
HYDB0Z7LAMINE HTDBOCHLOBIDE NH2(0H).HC1.
Solubility of each in Several Solvents.
(de Bruyn, xSga.)
Solvent.
r.
Gms. NJHUOH
per xoo (rms.
Solution.
f.
Cms. NH«(0H).HC
per xoo Gms.
Solvent.
Methyl Alcohol (abs.)
5
35
19-75
16.4
Ethyl Alcohol (abs.)
. ^5
IS
19-75
4.43
Ether (dry)
(b. pt.)
1.2
• • •
. . •
Ethyl Acetate
(b. pt.)
1.6
• • •
• ■ •
For densities of NHi(OH).HCl solutions, see Schiff and Monsacchi, 1896.
CO
PhthalylHTDBOXTLAMINE C«W*0 vtOH/^'
One liter benzene dissolves 0.33 gm. of the A form of melting point 220^-226^
(Sidgwick, 19x5.)
HTOSCYABONE drHnNO,.
Solubility in Several Solvents at i8?-22*.
(MOller. X903.)
Gms. CnHnNOk Gms. CnC^NOb
Sdvent. per xoo Gms. Solvent. per xoo (^ms.
Solution. Solution.
Water 0.355 Chloroform 100+
Ether 2 . 02 Acetic Ether 4 . 903
Ether sat. with H2O 3 .913 Petroleum Ether 0.098
Water sat. with Ether 3 . 125 Carbon Tetrachloride 0.059
Benzene 0.769
325 HTOSCmS
HYOSCINS (Scopolamine) HTDROBROMIDE, etc.
Solubility in Several Solvents at 25". (U. S. P. vm.)
Grams per loo Grams Solvent.
t * -^
Solvent. Hyofidne Hyoscyamine Hyoficnramine
Hydrobromide Hydrobromide Sulfate
CnHnN04HBr.3H,0. Ci7HsN0b.HBr. (Ci7HnNQ^,.H«SQ|
Water 66.6 very soluble very soluble
Alcohol 6.2 50 15.6
Ether ... 0.062 0.04
Chloroform 0.133 4^ oo43
Nitro INDAN Carboxylic Acids.
Freezing-point lowering data for mixtures of / nitroindan-2-carboxylic acid
and d nitroindan-2-carbozylic acid are given by Mills, Parker and Prowse, 1914.
CO
INDiaO (C(H4<^:„>C:),.
100 gms. 95% formic acid dissolve 0.14 gm. indigo at 19.8^ (Asdum, 1913.)
INDIITM lODATE In(IO,),.
100 gms. H2O dissolve 0.067 g™* In(IO|)i at 20^ (Mathers and Schluederbcig, 1908.)
IsoINOSITOL CeHisO..
100 gms. H|0 dissolve 25. 12 gms. CeHisOiat 18** and 43.22 gms. at ioo^(Mtt]]er,i9za.)
IODIC ^ ACID HIO,.
Solubility op Iodic Acid in Water. (Groscbuff. 1906.)
*•• lo^cSi'sit^Sol. Solid Phase. f. .SoiiftarSol. SoUd Phase.
— 0.3 1.69 Ice 16 71.7 mo*
— 1. 01 6.81 " 40 73.7 **
— 2.38 26.22 « 60 75.9 ••
— 4.72 51.42 « 80 78.3
— 6.32 57.61 « 85 78.7
— 12.25 67.40 " lOI 80.8
— 14 69 . 10 " +HI0i 1 10 82.1 fflOi+HIA
— 15 70 (unsuble)lcc 125 82.7 HIA
— 19 72 " '• 140 83.8
o 70.3 mo, 160 85-9
Solubility of Iodic Acid in Nitric Acid. (Groschuff.)
M
M
f.
Gms. HIOi per xoo Gms.
IODINE I2
Aq. 27. y% HNOs 40.88% HNOi
Solution. Solution. Solution.
o 74.1 18 9
20 75.8 21 10
40 77.7 27 14
60 80 38 18
Solubility of Iodine in Water. (Hartley, 1908.)
M Gms. I per looo Gms.
•• H,0.
18 0.2765
25 0-339S
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, 191 1; Herz and Paul, 1914 and Fedotieff, 1911-12.
lODINX
326
Solubility of Iodine in Aqxteous Mercuric Chloridb and in Aqueous
Cadmium Iodide Solutions at 25**.
In Aq. Cdli.
(Van Name and Brown, 1917.)
Gms. per Liter.
In Aq. HgCls.
(Herz and Paul, 19x4.)
.
Millimols per
Liter.
1.. '
Gms.
per Liter.
Hg.
HgCl,.
I. ^
0
1-34
0
0.340
94.44
12.94
25.64
3.28s
124.42
14.60
33.78
3.706
195.42
18.06
54.29
4.583
334.60
2$. 43
90.84
6.454
Cdl,.
L
3.66
2.072
45.78
9.056
91.56
11.386
183.12
14.040
Solubility of Iodine in Very Dilute Aqueous Solutions of Potassium
Iodide.
(Determinations made with very great care.)
Results at o^.
Cones and Hartman, 19x5.)
Results at 25". Results at 25**.
(Bray and MacKay, 19x0.) (Noyes and Seidenstricker, 1898.)
Normality
Gms. I per
Normality
Millimols If
Normality
Millimols I|
of Aq.
xoo Gms.
of Aq.
per Liter 1
Sat. Sol.
of Aq.
KlSd.
per Liter
KISoL
Sat. SoL
Sat. Sol.
KISol.
Sat. SoL-
0.000992
X.0002
0.0282
0
1.333
0
1.342
0.00200
1.0004
0.0409
O.OOI
1.788
0.00083
X.814
0.00500
I. 0010
0.0760
0.002
2.266
0.00166
2.235
O.OIOOO
X.0020
0.1356
0.005
3.728
0.00664
4.667
0.01988
1.0044
0.2S33
O.OIO
6.185
0.01329
8.003
0.0500
I. 0109
0.609
0.020
11.13
0.02657
4.68
0.09993
I. 0219
1. 199
0.050
25.77
0.05315
28.03
O.IOO
51-35
0.1063
55 .28
Solubility of Iodine in Aqueous Solutions of Potassium Iodide at
25** and Vice Versa.
(Parsons and Whittemore, 191 x.)
(Time of rotation 6 mos. or longer. Duplicate determinations at different lengths of time, were made.)
Sp. Gr.
Sat. Sol.
1.349
Gms. per 100 Gms.
Sat. Sol.
Solid
Phase.
Iodine
Sp. Gr.
Sat. Sol.
3.246
Gms. per
100 Gms.
Sol.
Solid
Phase.
KI
KI
16.03
I
18.49
KI
27.92
I '
66.45
1. 516
19.70
26.16
II
3.232
29.71
62.81
M
1.769
22.88
36.06
II
2.665
35.80
49.61
M
1. 910
23.55
40.52
II
2.539
38.09
44.58
M
2.403
24.78
53.60
II
2.216
44.82
31.01
M
2.904
25
63.12
It
2.066
49.04
23.08
M
3.082
25.18
66.04
11
1.888
54.41
11.63
II
3.316
26
68.09
" +KT
1.733
60.39
0
M
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 bv Parsons and Corliss.
iQio. 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
Ii/KI was found to be i or more in all cases. (See also p. 537.)
Freezing-point lowering data, determined by time-coohng 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
lODINK
Solubility of Iodine in Aqueous Solutions op Potassium Broiodb
AND OF Sodium Bromide at 25**.
(Bell and Buckley, 1912.)
In Aq. KBr
Solutions.
In Aq. NaBr Solutions.
bnift. KBr
Gm. Atoms I
Gnu. NaBr
Gm. Atoms I
per Liter.
per Liter.
per Liter.
per Liter.
60.6
0.0176
96.4
0.0266
106.9
0.0278
187.7
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
330 -6
0.0717
4991
0.0648
377-1
0.0797
569.9
0.0644
411
0.0864
632
0.0622
461.7
0.0948
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.
Aqueou&Add.
Mols. I per Liter
Sat.Sol.
Gms. I per Liter
Sat. Sol.
Authority.
o.ooinHCl
0.001332
0.338
(Bray and MacEay, i
o.ionHNQj
0.001340
0.340
(Sammet, 1905.)
o.ionH2S0i
0.001342
0.341
u
Solubility of Iodine in Aqueous Sodium Iodide Solutions.
(Gill, 1913-X4.)
A(}ueous 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
perxoocc.
Aq. Solution.
d»ot
Aq. Nal
Solution.
^ of Aq. Nal
after Satuiatkm
withL
Gms. I Dissdved
at 2S* per xoo Gnu
of the Sat. Sol.
5
10
IS
20
1.0369
1.0720
I. 1072
I . 1458
1.0698
I.I415
I. 2162
1.2998
4.99
9.96
14.93
20.02
Determinations at other temperatures were made in an apparatus which per-
mitted constant stirring of the solutioiis at the several temperatures. Results^
interpolated from the original, are as follows:
4«
Gms. I Dissolved
Sat. Solution in
per xoo Gms.
Aq. Nal of:
I^.
10 Gms. per
so Gms. per
xoooc.
xoooc.
10
8.9
17.6
15
9-3
18.3
20
9.6
19
25
10
19.4
Gms. I Dissolved per too Gms.
Sat. Solution in Aq. Nal of:
• .
10 Gms. per
so Gms. per'
zoocc
100 cc.
30
10.3
20.5
40
10.9
22
so
II. 7
23.4
60
12.6
24.9
lODINK
3^8
Solubility of Iodine in Aqueous Salt Scx^utions at 25*.
(McLauchlan, 1903.)
Sdt.
Cms. aat
Cms. Dinolved
Qalf
Gais.SiUt.
Gms. Dtaeolved
per Liter.
I per Liter.
.aait.
per Liter.
I per liter.
Na,SO«
29.77
0.160
NHiCl
53-4
0.73s .
K,SO«
435
0.238
NaBr
103
329
(NH4),S04
33
0.346
KBr
119
3.801
NaNO,
»5
0.257
NHiBr
98
4.003
KNOt
101.3
0.266
NH4C*HA
77.1
0.440
NHiNQi
80
0-37S
(NH«),C04
86.9
0.980
NaCl
585
OS7S
HiBQi
SS'^
0.300
KCl
73-6
a. 658
Solubility op Iodine in Nitrobenzene Solutions Containing Various
" Iodides at Room Temperature. Solutions Sat. with I in Each Case.
(Daweon and Goodaon, 1904.)
Iodide.
Cms. per Liter.
Iodide.
Iodine.
Potassium Iodide
12.35
112. 7
<( II
45.56
295 -7
M II
115.8
698.2
If II
•
155-2
943.6
Sodium Iodide
13.55
"5
II II
57.7
393
i« II
X09.X
738
U it
238
1251
Rubidium Iodide
85-4
421
Rubidium Iodide
217.5
X060
Lithium Iodide
S4.X
642
Iodide.
Caesium Iodide*
Caesium Iodide
Ammonium Iodide
Ammonium Iodide*
Aniline Hydriodide
Dimethylaniline Hydriodide
Tetramethylanunonium Iodide
Tetramethylammonium Iodide
Strontium Iodide
Barium Iodide
Barium Iodide
Gins.pa
Uter.
Iodide.
lodineu
48.2
213
223
858
69.5
482
94.3
669
164
721
160
6f6
49.3
266
51.4
280
106.5
,'>99
42.2
237
158.5
809
* Sdvent « 0 nitrotoluene instead of nil
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 Ethtl and Normal Proftl Alcohol
Solutions at 15*.
(Bniner, 1898.)
In Aq. Ethyl Alcohol.
r
Vol. %
dHiOH
in Solvent.
10
20
30
40
SO
Cms. I per
100 cc.
Solution.
o.os
0.06
O.IO
0.26
0.88
Vol. %
qiLOH
in NMvent.
60
70
80
90
100
Cms. I per
100 cc
Solution.
1. 14
2.33
4.20
7-47
15-67
In Aq. (n.) Propyl Alcohol.
\Jk
Vol.
in Solvent.
10
20
30
40
SO
Gms. Iper
xoocc.
Solution.
O.OS
O.II
0.40
0.94
1.64
Vol. %
CHjOH
insolvent.
60
70
80
90
100
Gms. Iper
xoooc.
Solutioii.
a. 71
4.10
6.05
9.17
14.93
3^
lODINS
SOLUBILITT OF lODINB IN AqUBOUS EtBYL AlCOHOL AND IN AqUBOUS ACBHC
Acid Solutions at 25**.
(McLauchlan, 1903.)
In Aq. CtHfOH Solutions.
Gms. CtH^H Gms. I per
per zoo Gma. xoo cc Sat.
Solvent. Sdutkxi.
o 0.034
455 0.039
28.48 0.172
44.41 0.9SS
72.51 6.698
100 24 . 548
In Aq. CHiCOOH Solutions.
Gms. Ijper
100 cc. Sat.
Solution.
0.034
0.076
0.173
0.510
3.162
Gms. CHt(XX)H
per 100 Gms.
Solvent.
O
20
39S
61. 1
80.7
100
Solubility of Iodinb in Aqubous Glycbrol Solutions at 25^
(Hers and Kooch, 1905.)
Density of glycerine at 25V4** "- 1-2555; unpurities about i.5%.
Wt.% Glycerine . MiUimcOs I
m Solvent, per xoo cc. Solution.
O
20.44
31 55
40.9s
48.7
69.2
100. o
0.24
0.27
0.38
049
0.69
1.07
2.20
9.70
Grama I per
zoocc.Solutioa.
0.0304
o .0342
0.0482
0.0621
0.0875
0 53S
0.278
1.223
Density of
Solutions at a5V4**
O
I
I
I
I
I
I
I
9979
0198
0471
0750
099s
1207
1765
2646
100 gms. glycerol (da "■ 1.256) dissolve 2 gms. iodine at I5**-I6^
(Ossendowski, 1907.) ^ ~
Solubility of Iodinb in Bbnzbnb, Chloroform, and in Ethbr.
(Arctowski — Z. anorg. Chem. xx, 376, *9S-*96')
In Benzene.
In Chloroform.
,
[n Ether.
^0 Gms. I per 100
* ' Gms. Soiutioa.
t«.
Gms. I per xoo
*•.
Gms. I per xoo
Gms. Solution. <
Gm^ Solutian.
4.7 8.08
-49
0.188
-83
15-39
6.6 8.63
-SSi
0.144
-90
14 58
10.5 9.60
-60
0.129
-108
IS 09
13.7 10.44
-69i
0.089
16.3 11.23
-73i
0.080
+ 10
1.76 per
100 gms.
CHCl,
S(m<ubility of Iodinb in BROiiOFCMtM, Carbon Tbtrachloridb, and in
Carbon Disulfidb at 25^
(Jakowkin, 1895.)
I liter of saturated solution in CHBri contains 189.55 fif^u. I*
I liter of saturated solution in CCI4 contains 30.33 gms. I.
I liter of saturated solution in CSi contains 230 gms. I.
lODINS
330
Solubility of Iodine in Carbon Disulfidb.
(Arctowiki, Z894.)
r.
Gms. I per xoo
Gms. Solutioo.
f.
Gms. I per xoo
Gms. Solutkm.
r.
[Gms. I per xoo
Gms. Solution.
— 100
- 80
0.32
0.51
0
10
7.89
10.51
30
36
19.26
22.67
- 63
1.26
IS
12.3s
40
25.22
— 20
4.14
20
14.62
42
26.7s
— 10
SS2
2S
16.92
Solubility of Iodinb in
Several Solvents at
25^
Solvent.
Iodine per Liter of
Sat Sol.
Solvent.
Trichlorethylene
Tetrachlorethane
Pentachlorethane
Iodine per Lher d
Sat. Sol.
Mols.
Chloroform 0.352
Carbon Tetrachloride 0.237
Tetrachlorethy lene 0 . 24 1
Gms.
44.68
30.08
30.59
' Mols. Gms. '
0.312 39.61
0.244 30.97
0.272 34.53
One liter sat. solution of iodine in nitrobenzene contains 50.62 gms. I at 16^-17*.
(Dawson and Gawler, 1902.)
100 gms. hexane dissolve 1 .32 ^ms. iodine at 25**. (Hildebcand* Ellefson and Beebe, 19x7.)
100 gms. sat. solution of iodme in anhydrous lanolin (melting point 46^), con-
tain 5.50 gms. iodine at 45^. (Klow, 1907.)
Solubility of Iodine in Mixtures of Chloroform and Ether at 25^
(Maiden and Dover, 19x6.) 'j
Cms. CHCla per xoo Gms. Iodine per xoo Gms. CHC% per xoo Gms. Iodine per 100 Gmi.
Cms. CHa«+(^H|)A Gms. CHC1,+(C|H|)A Gma. CHC1,+(&H|)A CHC1,+(CA}A
60 9.83
70 7S
80 S-73
90 431
100 3.10
100 cc. of a mixture of CHCU •+• CS| (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, 191 1: CHIs, p C«H4Brt, [CsHilNs, p C«H4(N0i)i»
(CeH»CO),0 and C«H»COOH.
0
3SI
10
29.6
20
24.8
30
20.2
40
16.3
so
• 12.7
S(H.UBILITY OF lODINE IN MiXBD SOLVENTS AT l6.6^.
Solvent.
Ether
Carbon Disulfide
Ether+3.96 gms. H|0 per liter
4- 7.91 gms. HiO "
-j-cxcessHiO
+9.79 gms. CiH»OH "
-I-I9-6
+29.4
+39-2
ti
it
<f
it
«
tt
tt
tt
tt
tt
tt
tt
tt
(StrOmholm, 1903.)
Gms. I
per Liter
Sat. Sol.
206.3
178. S
221
Solvent.
Ether +20.96 gms. CS| per liter
Ether-l-41.9
CSi -1-22.5
235.7 CSt +45-1
251.4 Ether+47.63
219. 1 CSi 4" 50.06
231.5 Ether-l-80.3
243.9 Ether-I- 77-85
254.4 CSf +62.2
It
tt
tt
tt
tt
tt
It
tt
CSi
ether
ether
CHCU
CHCU
CiHs
CHiI
S
If
<i
If
11
If
II
II
If
Gms. I
per Liter
Si^.Sol.
202.3
217.2
189.3
20X.X
195.2
172.8
204.x
220.2
18^4
One liter sat. solution in ether contains 167.3 i^ms. I at o^ (StrAmholm, 1903.)
aai lODINS
SOLUBILITT OF lODINB IN MIXTURES OF CHLOROFORM AND EtHTL AlCOHOL,
Chloroform and Normal Propyl Alcohol, Chloroform and Benzene,
AND Chloroform and Carbon Disulfide at 15**.
(Bruner, 1898.)
% (:H(a,
Solvent.
Cms. I Dissolved per 100 oc. of Miztuies of:
CHCU+C|H»0H.
CHCU+C^tOH.
CHCla+CA.
chcu+cs^
0
15-67
14.93
10.40
17-63
10
9-43
13 16
9.84
iS-93
20
8.69
11.20
8.78
14.20
30
7.80
8.98
7-74
12.16
40
7.09
8.09
6.96
10.20
SO
6.62
7.82
6.20
9.08
60
6.24
7.09
534
7.72
70
577
6.42
4.89
6.42
80
506
554
453
S.27
'90
4.34
4.52
4.07
4.32
100
3.62
3 62
3 62
3 62
SOLUBILITT 07 lODINB IN MIXTURES OF CaRBON TETRACHLORIDE AND BEN-
ZENE AND IN Mixtures of Carbon Tetrachloride and Carbon Disul-
fide AT 15". (Bnmer. 1898.)
Vol. 7 CCL ^™** ^ I*^ ^^'* ^' ^ ^<Ii3ctuxe of: y^i m qqi Cms. I per 100 cc. of Mixture of:
"^^^*- ' CCI4+CA. CCU+CSi. ' insolvent. 'cCU+CA. ' CCI4+CS,.'
o 10.40 17.6 60 4.90 S'SS'
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 8.60 100 2.06 2.06
SO S.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 Disulfide, and Water and Carbon Tetrachloride at 2S^
aakowkin, 1895)
The origind results were plotted on cross section paper and tlie foUowin^ table made from the corvei.
Jakowkm points out that the resuha of Bcrthelot and Jungflebch, xSya, are.inooixect on account of the
pieiwnos 01 n^r
Gnu. I per Liter
of H«0 Layer
faiEachCMe.
Cms. I per Liter of-:
CHBr,Uyer.
CS| Layer.
CCIiLajrtr
o.os
20
30
4
O.IO
4S
60
8.5
o.iS
71
91
13
0.20
100
126
17s
0.2s
130
160
32
A theofetical diecusuon of the results of Jakowkin is given by Schakarew (1901).
lODINB
33^
DisniBunoN of Iodinb bbtwbbn Carbon Disulfide and
Aq. Potassium Oxalate.
(DiiracB— Z. phyA. Cbem. s6» '6101 '06; Dewbod and McRae — J. Cbem. Soc. 8x, 1686, 'et^
CoBcentntiflO
of
Aq. KsCiQft.
i.o Equiv.
I .0
I .0
1.0 "
1.2 "
Gma. I pa
Liter of
Aq. Layer.
2.408
CSsLayer^
10.82
3SSS
5.766
6.861
16.32
27.91
34.01
3 525
17.07
Vol. of Solutkn
which Contains
I Mol. I.
105.3
71 -37
43-99
36.98
71.97
Fraction of I
Uncombined
in Solution.
0.00549s
0.00561
o 005915
0.006055
0.005645
Distribution op Iodine between Amyl Alcohol and T/ater and
BETWEEN Amyl Alcohol and Aqueous Potassium Iodide
Solutions at 25**.
(Hen and Fischer — Ber. 37, 4753, '04.)
The original results were plotted on cross-section paper, and the
following tables made from the curves.
Mmixnols I per XO cc
Amyl Alcohol Layer
in Each Case.
•/
HjO.
Nki.
xo
XO
XO
10
10
2S
0.012
0.13s
0.160
0.170
0.170
• • •
30
0.014
0.150
0.185
0.200
0.200
0.160
4.0
0.018
0.180
0.235
0.255
0.270
0.240
s
0.021
0.210
0.280
0.315
0.340
0.315
6
0.025
0.230
0.330
0.37s
0.410
0.390
7
0.029
0.250
0.37s
0.430
0.480
0.470
8
• ■ •
0.260
0.420
0.490
0.550
0.555
9
• • •
0.270
0.450
0.550
0.620
"
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
• • •
• • •
O.S75
• • •
• • •
• • •
G1M.I per 100 cc.
Cms. I pel
' xoo cc. of HsO and of KI Layers.
Amyl Alcohol Layer
inBachOMB.
HaO.
Nki.
xo
XO
xo
XO
loN
10
!n.
3
0.014
0.164
0.20
0.21
0.21
■
• ■
4
^; 016
0.196
0.24
0.26
0.26
0
.31
6
W.026
0.252
0.34
0.38
0.40
0
•37
8
0-033
0.297
0.43
0.49
0.54
0
•SI
10
0.040
0.328
0.51
0.61
0.67
0
.69
12
0.341
0.58
0.73
0.81
0
.84
14
« • •
0.60
0.83
0.95
I
.00
16
• • •
0.63
0.91
1.09
I
• 30
18
• • •
0.64
• • •
• • •
•
• •
2S
• • •
0.71
• ■ •
• • •
•
• •
The original figures for 5N/10 and loN/io KI solutions give prae«
tically identical curves.
Results for the distribution of Iodine between N/io KI solutions on
the one hand, and mixtures in various proportions of CeH«+ CS,,
CeH,CH,+ CS„ CeHe+CeH.CH,, CeHe +liglit petroleum, CS,+ light
petroleimi, CS,+CHC1„ CHC1,+ C^H., CCI4+ CS, and CCI4+ CeH.CH,
on the other hand, are given by Dawson — J. Chem. Soc., 81, 1086, 'oa.
333
Distribution of Iodinb between Water and IioasaBLQ Organic Solvenisl
Results for Water Results for Water Results for Water Results for Wator
+ Nitrobenzene + Carbon Disul- + Chloroform
at I8^ fide at I5^ at 25^
(DaivBOD, 1908.) (Dawaon, z9oa.) (Eben & Knner, 1910}
Mob. Iodine per Liter. Cms. lodiae per liter. Mob. Iodine per liter.
+ Carbontetra-
chloride at I8^
CDawaon, 190S.)
Mob. Iodine per Liter.
HdOUyer. CCULayer. &^ Layer. CANOiLayer:ByO Layer. CSiLayer. H|0 Layer. CHCliUyoB.'
0.00019 0.0333
0.00050 0.0854
0.00133 0.2275
0.00189 0.3328
Results for Water
+ Tetrachlor-
ethylene at 25^.
0.0452 27.85
0.0486 30.09
0.0486 30.31
Results for Water
-h Tetrachlor-
ethane at 25^
0.00025 0.0338
o.ooxao 0.1546
0.00x84 0.23x8
0.00259 0-3439
Results for Water
+ Pentachlor-
ethane at 25^
0.000416 0.0344
0.000535 0.0443
Results for Water
4- Trichlorethyl-
ene at 25^
(HenftRathmann/ij.) (HeR&Rathmann,/x3.) (Hen^Rathmann,'!^.) (Hen&Rathiiiann,'z3^
Mob. Iodine per Liter. Mob. Iodine per Liter. Mob Iodine per litfer. Mob. loctine per Liter.
' 55 cHa.ca. ' 55 cOi-cci, H^o oHsCU ' 5o CiHCur
Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer.
0.00046 0.0543 0.00088 0.0653 0.00119 o.iiox 0.00092 0.0848
0.00070 0.0778 0.00127 0.0932 0.00145 0.1247 O.00117 0.X067
0.00x12 0.1275 0.00172 0.1285 0.00159 0.X479 0.00160 O.X434
0.00236 0.2672 0.0028X 0.2161 0.00217 0.2103 0.00204 0.1963
Data for the distribution of iodine between water and mixtures of CS|+CC1«
at 25^ are given by Herz and Kurzer, 191 o.
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.
191 7. Cadmium iodide, cadmium potassium ioidide, lanthanum iodide, nickel
iodide, strontium iodide, zinc iodide and 7inc potassium iodide. Results for the
distribution of iodine between carbon tetrachloride and aq. mercuric potassium
iodide are also ^ven.
Results for distribution between CS| and aq. Bali sols, are given by Herz and
Kurzer, 19 10.
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 Hers
and Paul, 1914.
Distribution of Iodine between Carbon Distxfidb and Aq.
Ethyl Alcohol at 25"". (Ouka, 1903-08.)
Gms.aHiL0H Gms. Iodine per Liter:
c
Gms. CiHiOH
Gms. Iodine per Liter:
per 100 cc. tis, T Ayer Aq. Alcohol
Aq. AloAoL c. Layer c*.
?•
per 100 oc
Aq. AloohoL
CS| Layer Aq. Alcohol p*
e. Layer c'.
7.6 0.072
35.86
0.0020
19. 1
0.330 97 0.0034
7.6 0.2IZ
107.79
0.0020
22.9
0.II5 23.78 0.0048
II. 4 0.077
32.93
0.0023
22.9
0.413 89.61 0.0047
II. 4 0.280
133 -22
0.0021
26.7
0.0756 9.8 0.0077
15-3 007s
25.61
0.0029
26.7
0495 65.10 0.0076
iS-3 O.31S
"534
0.0027
30.5
0.0636 4.90 0.0130
19. 1 0.045
13.42
0.0034
30.S
0.546 42.27 o.oiag
Distribution of Iodine between Ether and Ethylene Glycol. (Landau, 1910^
Results at o^
Results at 25^
Gms. Iodine
per Liter:
m
Gms. Iodine per Liter:
lAyer (^.
£^^!"
V
^U
. i^^! *•
2.139
1.449
1.48
2.208
1.449 1.52
7.820
4.347
1.80
4.255
2.541 1.60
16.620
9.486
1.75
7.728
4.347 1.78
20.564
11.685
1.76
16.200
9.120 1.78
31 . 785
18.135
1.7s
30.322
17.062 1.78
79.950
44460
1.80
78.19s
44.4^ 1.76
lODINB
334
Distribution of Iodine BvtwsBs Glycerol and Benzene and between
Glycerol and Carbon Tbtrachloridb.
(Landau, 19x0.)
Results for Glycerol and Benzene.
f.
u
it
u
ii
40*
«
ii
ii
ii
so'
ii
ii
ii
ti
Gtami Iodine per Liter;
Glycerol Layer. Beniene Layer.
(«)
0.407
0.676
1.470
2.622
S*28o
0.4S9
0.658
1.584
3.048
5564
0.467
0.642
1.463
2-391
5-383
(*)
1.922
4.086
10.212
20.102
42.458
2.168
3-9"
11.244
24.104
46.960
2.194
3.864
II. 196
19.872
46 . 782
(a)'
4.72
6.04
6.95
7.67
8.04
4.72
5-94
7.10
7.91
8.44
4.70
6.02
7-65
8.31
8.69
25
<
<
40
so
Results for Glycerol and CCU.
Gma. Iodine per Liter;
Glycerol Layer. CCI4 Layer!
(a)
0.365
0.684
1. 416
5.064
7.636
0.322
0.690
1.224
2.832
6.854
0.299
0.570
1.5"
2.664
6.348
(ft)
0.56s
1.224
2.652
9.888
14 . 766
0.575
1. 169
2.772
6.444
15.410
0.653
1.270
3-457
6.468
16.008
21
(«)'
1.5s
1.78
1.87
1-95
1-93
1.79
1.74
1.69
2.26
2.25
2.19
2.23
2.29
2.43
2*52
Distribution of Iodine between Glycerol and Chloroform.
Results at 25*".
(Hen & Kuner, 1910.)
Results at 30"*.
(Hantach & Va(t, xgoi.)
Results at Dif. Temps.
(Hantach & Vagt, 1901.)
Mda. Iodine per 1000
Gms.
Glycerol
Layer c.
0.0244
0.0397
0.0500
CHCU
Layer c'.
0.0564
0.0919
0.1151
e
c'
0.43
0.43
0.43
Mob. Iodine per Liter;
Glycerol
Layer c.
0.00097
c
c'
CHCU
Layer c,
0.00172 0.056
0.00204 0.00412 0.495
0.00418 0.00898 0.465
0.00782 0.0216 0.362
f.
O
20
40
SO
Mob. I per Liter:
Glsrcerol
Layer c.
0.0119
0.0084
0.0077
0.0074
CHCU
Layer tf*.
0.0177
0.0213
0.0221
0.0226
N -•
e
?
0.675
0.400
0.349
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 C^lycercx. and Ethyl Ether.
(Hantach & Va(t, 1901.)
Mob. Iodine per Liter:
f.
O
30
30
Glycerol Layer
0.00566
0.00544
O.OOIOO
Ether Layer
(O.
0.0270
0.0272
0.0051
c
0.21
0.20
0.20
FREEnNG-roiNT Data (Solubility, see footnote, p. i)for Mixtures op
Iodine and Other Elements.
Iodine and Selenium
" Sulfur
" TeUurium
" Tin
(Pelllni and Pedrina, 1908.)
(Olivari, 1908; Smith and Canon* 1908.)
(Jaeger and Menke, 19x9.)
(van Klooster, 1919-13; Remden and de Lange, 1919-13.)
Solubility of Iodine in Arsenic Trichloride. (Sk»n and Maiiet, 1889.)
f. o*. IS*. 96*.
Gms. I per loo.gms. AsCU 8.42 11.88 36.89
335 lODOIOSnOB
lODOIOSIN (Sodium tetra iodofluorescein) CwHeliOsNas.
lOO gms. HiO dissolve 90 gms. iodoeosin at 20-25^ (Dehn, 1917O
100 gms. pyridine dissolve 4.63 gms. iodoeosin at 20-25^ '*
100 gms. aq. 50% pyridine di^olve 71.6 gms. iodoeosin at 20-35^ "*
lODOFOBM CHI,, lODOL C4I4NH (Tetraiodopyrrol).
Solubility in Several Solvents.
(U. S. p. Vni: Valpins, 2893.)
Gms. per 100 Gms. SolveaL
owvcnt.
• .
CH,I.
C«I«NH.
Water
25
0.0106
0.0204
Alcohol
25
2.14 (1.43 gms. (V.))
II. I
Alcohol
b. pt.
(10 gms. (V.))
...
Ether
25
19.2 (16.6 gms. (V.))
66.6
Chloroform
25
• • •
0.9s
Pyridine
20-25
173. 1 (Dehn. 1917.)
Aq. 50% pyridine
20-25
22.4 "
Lanolin (30% HiO)
46
5.2 CKkee.1907.)
ntlDIUM CHLOBIDI IrCU.
When I gm. iridium as chloride is dissolved in 100 cc. of 10% HCl and shaken
at 18^ with 100 cc. of ether, 0.02 per cent of the metal enters the ethereal layer.
When 20% HCl b used 5% of the metal enters the ether. When dissolved in i %
HCl or in water approximately 0.0 1 per cent of the metal enters the ethereal layer.
(MyUos, 1911.)
ntlDIUM Ammonium CHLOBIDI IrCU.2NH4Cl.
SoLUBiLrrY IN Water.
(Rimbftch and Kotten, 1907.)
Gms. ItCU.sNH|C1 per 100 Gms.
*•. t * \
Water. Sat. Sol.
f.
Gms. IrCl4.aNH«Q per 100 Gms.
Water. Sat. Sol.
14.4 0.699 0.694
522
1.608 1*583
26.8 0.905 0.899
61.2
2.130 2.068
39.4 1.226 I. 124
693
2.824 2.746
IRIDIUM DOUBLE SALTS.
Solubility in Water.
(Palmaer — Ber. 23, 3817; 34* aogo, '91.)
Doable Salt. Formula.
Irido Pentamine Bromide IrCNHJsBr,
" " Bromonitrate Ir(NH,),Br(NOJ,
" « Trichloride Ir(NH,).a,
" « Chloro Bromide Ir(NH,).ClBr,
" *' Chloro Iodide Ir(NHj4ClI,
" " Chloro Nitrate Ir(NH,),a(NO.),
•* " Chloro Sulphate Ir(NH,),CIS04.2H,0
•* " Nitrate Ir(NHJ,(NO,),
'' Aquo Pentamine Bromide Ir(NHi)«(OH^Br,
" ^' " Chloride Ir(NH,).(OH,)Cl,
" •' " Nitrate Ir(NH,),(OH,)(NOJ.
IBOV BBOMIDE (Ferrous) FeBr2.6H,0.
Solubility in Water.
(Etard — Am. chim. phys. [7] a, 537, '94.)
A« Gms. FeBf^
per 100 Gms. SoL
—20 47 O
O SO. 5
ao S3S
t*
Gms. per too
• •
Gms. H^.
"5
0.284
18
5-5B
15. X
6.53
15
0.47
15
0-95
15-4
1.94
150
0.74
16
0.28
ord. temp.
25.0
Old. temp.
74.7
17
10. 0
t».
Gms. FeBh
per 100 Gms. SoL
t».
Gms.FeBiiL
per 100 Gms. SoL
30
55 0
60
590
40
56.2
80
61.5
100
64.0
IRON CARBONATE
336
IRON CARBONATE (Ferrous) FeCOs.
Solubility op Ferrous Carbonate in Aqueous Salt Solutions, Both
WITH AND without THE PRESENCE OF CaRBON DIOXIDE.
(Ehlert and Hempel, 19x2.)
(Each mixture was 1000 cc. in volume and was rotated constantly for 24 hours.
Temp., probably 5-8**.)
Solubility in
Presence
S(M.UBILITY
in Absence
OF C0| (a atmospheres pKssure).
Gnu. Salt per Gms. FeCXH per
OF
CO,.
Aqueous Sdotion oC:
Cms. Salt per
1000 Gm. BiO.
Gms. FeCOk per
xooo Gms. H^.
xooo cc. Solveat.
xooo oc. Solvent..
Water alone
0
6. 191
• • •
• • •
NaCl
• • «
• • •
3SI-2
0-350
MgCb.6HiO
86.9
S.«40
...
((
700
4SSS
. • •
U
1150
4-459
...
it
1437 s
4693
...
u
1725
5-398
• * •
it
2300
9.052
2300
4.205
Na»S04.ioH,0
137-7
7-943
137.7
0.701
<c
Sat. at 14**
9-578
Sat. at 14^
0.934
MgS0«.7H»0
105.3 ^
6.342
105.3 ^
1.467
C<
Sat. at 14^
7-392
Sat. at 14**
2.933
IRON BICARBONATE (Ferrous) Fe(HCO,)s.
SCX.UBILITY OF Ferrous Bicarbonate in Carbonated Water at 30^
(Smith, H. J., X9x8.)
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 lbs. 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 COi 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 ot the
saturated solution for analysis was withdrawn through a brass tuoe 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. HfSOi. The COa was determined by absorption and the iron by precipitation,
resolution, reduction* and titration with permanganate. The results show that
the decomposition tension of Fe(HCOt)t is greater than 25 atmospheres at 25^.
Gms. Mob
1. per Liter.
Fe(HCQi);.
Gms. per Liter.
Gms. Mob
H,C0,.
[. per Liter.
Fe(HCOa),.
Gms. per Liter.
HiCQi.
HsCOft.
Fe(HCO^i.
H,CO».
FeCHCO,),.
0.1868
0.00245
11.58
0.436
0.3294
O.OO3II
20.43
0.553
0.1985
0.00256
12.31
0.4S5
0.3745
0.00315
23.23
0.560
0.2168
0.00262
13.45
0.466
0.4046
0.00332
25.09
0.590
0.2327
0.00274
14-43
0.487
0.4750
0.00348
29.45
0.619
0.2960
0.00303
18.3s
0.539
0.6600
0.00402
40.93
O.71S
O.3I16
0.00304
19.32
0.541
0.7154
0.00418
44.36
0.744
0.3153
0.00318
19. 55
0.566
0.7600
0.00434
47-13
0.772
IRON CHLORIDE (Ferrous) FeCl,.4H,0.
100 gms. sat. sol. in water contain 17.54 R^^s. Fe
100 gms. sat. 80I. in water contain 18.59 S^is. Fe »
39.82 gms. FeCli at 22.8*.
42.8 gms. FeCli at 43.2^
(Boecke, xgxzO
337
IRON CHLOBIDI
ntON OHLOBIDB (Ferrous) FeClt.4H,0. Solubility in Watbr.
(EtaidO
Gins. FeCb
t*. periooGmB.
Solttdoo.
lo 39.2
15 40.0
25 41 S
30 42 -2
40 43.6
SO 45 •«
Solid Phase.
FcCla.41^0
a
tt
ti
a
u
Gms. FeOt
t*. per xoo Gms.
Sdutkn.
60 47.0
80 50.0
87 51.3
90 51-3
100 51.4
120 51.8
Solid Phsse.
FeCl,.4HaO
i(
FeCl,.4^0+FeCL
FeCl,
It
it
Solubility op Iron Chloride
(Rooseboom — Z. physik.
Mob. Ferfae ^^' ^^ P» »<»
»•. periooMdft. Gam.
HsO. go SdlntiaD.
Solid Phase, Fe|Cl«.zsHsO.
2.75
2.98
(Ferric) Fe,Qe in Water.
Oiem. 10^ 477, '93.)
Mob. FeaOft Gms.Feaaperioo
Mob.
Gms.
rfjol Solution.
Solid Phase, FeaC3e.5B^ (col).
per xoo_
HaO.
-55
-27
O
+ 20
30
37
30
20
8
49-52
53 60
74.39
91.85
106.8
150.0
201.7
231. 1
246.7
413
5.10
5-93
8-33
11.20
12.83
13 -7
Solid Phase, Fe]Cl6.7HsO.
20 11.35 2044
32 13 -55 2440
30 15.12 272.4
25 15.54 280.0
Sdid Phase. FesOe.sHsO.
12 12.87 231.8
27 14.85 267.5
33
34
42
47
51
60
66
69
71
67
70
73
73
69
72
12
93
66
88
64
01
85
79
IS
14
92
13
69
87
78
35 15.64 281.6 73
SO 17-50 315-2 75
55 19-15 344-8 77
55 20.32 365.9 78
Solid Phase, FesCl«.4HaO.
SO 19 -9^ 359-3 78
55 20.32 365.9 78
60 20.70 372.8 78
^ 21.53 387.7 79
73-5 25 o 450-2 81
70 27.9 502.4 83
66 29.2 525.9 84
Solid Phase, FesCI».
66 29.2 525.9 84
75 28.92 511 .4 83
80 29.20 525.9 84
100 29.75 535-8 84
79
9«
S«
54
23
54
86
SO
8x
41
03
03
66
03
26
Solubility op Ferric Chloride in Aqueous Solutions of
Ammonium Chloride at 25®, 35*^, and 45**.
(Mohr — Z. physik. Chem. 37, 197, '98.)
Results at 25^.
Restdts at 35°.
Resialts at 45^
Mob
• Der
Mob
Der
Mols
Der
100 Mob.' HgO.
Ua4Ci, FeCU.
xoo Mols. HjO.
NH«a. Fea,.
zoo Mob. HsO.
NH«a. Fea^
Solid Phase
in Each Case.
0
10.98
0
13-30
0.0
33-4
Feide-isHjO (sJHjO at 45")
1-57
10.74
1. 41
13 OS
• «
1 •
• • •
Hydnte-f Doable Salt
2.48
9.02
3.08
9.28
4
08
958
DoobbSalt
5.28
7-73
6.98
7.64
• t
1 •
• • •
M
9-59
6.77
10.76
6.70
13
09
6.31
U
983
6.70
11.60
6.52
13
54
6.28
DoaUe Salt + Mixed Ciyttab
9-65
6.07
12.28
6.08
13.
91
5-49
MuBed C^yitab
9-93
5-23
"•57
398
13
49
4.84
«
9.92
3-97
11.89
3-38
13
.46
4.99
«
10.31
2.05
13-23
1.38
•
1 •
• • •
«
13 30
0.0
14.79
0.0
16
.28
0.0
NHiQ
IRON CHLOBIDI
338
Solubility op
Pbrric Chloridb in Aqubous Solutions or
Ammonium Chloridb at ij;^.
- Z. phyak. Ch.
lOb 148, VaO
Mob. per 100
Mols.H/).
FeClt.
Gnzna per 100 Gma.HiO.
SaUd
NH«a.
NH4a.
FeCW
Phase.
0.0
9 30
00
83.88
Fi^«CU.iaH^
Z.09
957
3
24
86.32
M
1.3^
9-93
4
■03
91.61
Feia«.iaHsO + Double Salt
2.00
9.27
S
.92
83.64
DoabbSalt
2.79
8.71
8
■31
78.77
M
40s
8.09
12
.08
73.20
«
6.41
7.18
19
.12
64.83
M
10.78
6.21
32
.04
56.00
«
7.82
6.7s
23
.21
60.83
Mixed Cnritab mntitnhig 7.09% FcOi
7.62
S-94
22.
63
53-47
5^5 -
7.70
503
22.
90
45-42
44
7.81
4-34
23
23
39-13
SA
8.52
2.82
25
33
25-43
- - ,^ «
10.9s
0.68
32-
55
6.15
- • 041 •
11.88
0.0
35-
30
0.0
NHiQ
Solubility op Pbrric Chloridb in Aqueous Hydrochloric Acid
Solutions at Diffbrbnt Tbmperaturbs.
(Roozeboom and Schrdnemaker — Z. physik. Chem. 15, 633, '94.)
Mob
. per ic
1^,
100 Mob.
Gms. per 100 Gma.
HgO.
Ha.
O
7.52
13.37
z6.8o
18.45
20.40
20.10
19.95
19.00
18.05
18.05
19.50
24.12
26.00
26.00
3460
37.27
34.60
0.0
2.33
0.0
0.0
2.33
7.50
0.0
FeCls. HCl.
Results at o^.
8.25 O
6.51 15.22
6.SS 27.06
8.70 33.99
10.23 37.34
15.40 41.28
16.00 40.67
17.70 40.37
22.75 38.45
23-41 36.53
23.40 36.53
25.93 39-55
30.04 48.81
32.16 52.60
32.16 52.60
38.11 70.01
36.60 75.41
38.11 70.01
Results at a^.
10.90
23.72
24.5
23. 5
23.72
29.75
31-50
0.0
4.715
0.0
0.0
4.715
15.18
0.0
Fea«.
74- 30^
58.62
57 01
78.34
92.10
138.7
144. 1
159.4
204.8
210.8
210.8
233-5
270.5
289.6
289.6
343.2
329.6
343.2
Solid
Phase.
Mob. per xoo Mob. Gms. per 100 Gma.
H^. H«0. Solid
,Fc.Cla
.xaHaO
SoT
0.0
7.5
19-5
19-5
20.6
31-34
33- 00
34- 65
40.41
FeCb-
^HfO
FcCI». HQ.
Results at as** (coo.).
29.00 0.0 261. 1
29.75 15.18 267
35.25 39.46 317
35.25 39.46 317. 4^
35.34 41.68 318.3
41.58 63.42 374.4
66.77
70.11
81.77
78.98
72.33
Phase.
■j}'-^
o
13.4
^*^^i3.4
FeiCle *7.0
.aHa O
98.15
213
220
211. 6
213
267
283.6
.151 -_^ 42.50
•6 r?Sao 42.01
.7 J
43.00
44.80
40.25
39.03 41.38
35.74 45.24
Results at 40®.
32.4 0.0
37.45 27.11
37.45 27.11
50.80 54.64
58.0 0.0
27 50.8 54.64
42.01 48.64 85.00
47.52 86.72
48.64 85.00
387-3
403.4
362.4
372
407
■'-^
.and
4HtO
%SHjO
^*^jO
291.7
337.3
337.3
457.5
522. 31
457.5 ^ ^"^
438. oj
438.0) +4Hi0
Restilts for other temperatures
are also given in ^e original
paper.
339
IRON CHLOBIDI
Results for tbb Ststbm Ferric Oxide» Hydrochloric Acid, Water at 25^
(CajQfiiQn and Robinson* 1907.)
(Excess of ferric hydroxide was added to aq. ferric chloride solutions and agi-
tated for 3 months.)
Gnu.
FciOb.
34.61
33.27
32.78
31.9s
34.42
35-22
34.07
34.21
34-44
33.04
24.42
100 Gms.
.Sol.
—ficT
S9.88
60.23
5471
58.20
Solid Piiaae.
FeC\.HCLaB^
M
n
+ Fea«
FeCli+FeCI|.aB^
59 28
55-71
55. 47
51. II
46.72
33.40
M
U
U
+FeCI|.9iB^
FeCW.3iH|0+ "
" +FeCU.6H^
FeCW-SB^
dud
Sat.SoL
1.48s
1.349
1. 321
1.284
1.242
1.220
1. 19s
1.158
I. IIS
1.070
1.047
Gms. per 100 Gins.
SS.
Sol.
Solid Phase.
FeiOb.
21.84
16.82
15.83
14.62
12.59
11.76
10.56
8.60
6.47
4.04
2.85
M
M
I*
HCL
22.55 FeJOtjeaClSfi
21.10
19. S3
16.61
15.28
13.76
11.24
8.39
5.36
3.66
Data for the systems FeCU + MgCli + KCl -|- HiO at 22.8* and for FeCIt +
KCl + NaCl are given by Boeke, 191 1.
100 gms. abs. acetone dissolve 62.9 gms. FeCU at 18^. (Naumann, 1904.)
100 gms. anhydrous lanolin (m. pt. about 46®) dissolve 4.17 gms. FeCU at 45^
(Kkse, 1907.)
DiSTRiBonoN OF Ferric Chloride between Water and Ether at I8^
(Mylius, 19x1.)
One-gram portions of iron as chloride were dissolved in 100 oc. 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
Per cent of lion Extracted by Ether
I
(0.01)
5
o.i
10
8
IS
92
20
99
Fusion-point curves (solubility, see footnote, p. i) for mixtures of FeCli -f PbClt
and FeCls + ZnCls are given by Herrmann, 191 1, and for mixtures of FeCU+TlCl
by Scarpa, 1912.
SoLUBmrry of the Salt Pair FeCU-NaCl in Water at 21*.
(ICnzicfasen and Sachsd, 1904-05.)
Gms. Used.
Gms. per 100 Gms.
Solution.
G.
per xoo
FeOa.
Mols.
Mo]s.H^.
NaCL
Solid Phase.
FeCla.
NaCi:
Feci,.
Naa.
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
5.5
2
26.40
5.25
2.93
2.54
7.2
IS
38.15
390
4-23
1.22
9
I
45 38
2.45
5.03
0.75
10.8
o.S
46.75
2. II
5.18
0.65
10.8
0
83.39
0
9-3
0
FeCb
IRON CHLOBIDI 340
S(X.UBiLiTY OF THB Salt Pair FeCk-KCl IN Water at 2I^
(Hinrichsen and Sachael, 1904-05.)
I«t«n. fTsMl
Gnu. per
100 Gms.
Gms. Mob. per 100
\nilaa VMJa
Solution.
Mols.
H,0.
Solid Phase.
FeCU. KCL'
FeO^
KCl.
FeCU.
KCL'
0 35
0
34.97
0
8.45
KCl
13 28
13 -44
24.45
1.49
5.90
Mix Crystals
18 31
23.18
16.54
2.57
3-99
ti
23 18. s
28.05
11.69
3."
2.82
n
38 16
35-72
11.68
3-0
2.82
u
31 IO-5
36.62
II. 19
4.06
2.70
Fecu.2Kcl.H20
36.3 9
37-35
13.67
4.14
3.30
«
46.5 6
SI. 69
7.54
5.73
1.82
u
155 0
83.89
0
9.3
0
FeCU
Solubility of the Salt Pair FeCU.CsCl in Water at 21^
(H. and S.)
Gmi.
Vwd.
Gnu. per xooGms.
Solution.
Gms. Mols. per 100
Mols.H^.
FeCl,. CsCl.
Solid PiMse.
FeCU.
CsCL
FeCU-
CsCl."
0
0.6
1-4
65
II. 6
10.2
0
0.45
2.1
6s
SS-iS
52.38
0
o.os
0.23
6.95
5.9
5.6
CsCl
FeCU.3CsCLHiO
2.2
2
8.8
7.4
5-24
7.8
51.44
47.70
0.57
0.86
55
5.1
FeCU-sCsCl IW)
3-8
6
8.93
41.15
0.99
4.4
<(
4.6
5-4
6.3
4.6
2.8
1.4
15.34
21.6s
27.96
25 -25
14.96
8.45
1.70
2.40
3.10
2.7
1.6
0.9
il
U
35
35
0.2
0
48.71
83.89
0.94
0
5 -40
9-3
0.1
0
u
FeCli
IRON FOBMATE (Ferric) Fet(OH)s(HCOO)7.4HtO.
Solubility in Water and in Absolute Alcohol.
(Hampshire and Pratt, 19x3 •)
Solubility in Water.
Solubility
in Aba. AloohoL
Gms. Salt
Gms. Salt
f.
per xoo Gms. Solid Phase.
f.
per xoo Gms.
H,0.
ORfifEL
IS
S.08 Fei(OH)2(HCOO)7.4HiO
19
'4. 59
20
5.52 "
22
6.25
25
6.10
23
7.62
30
^7 ,< (The sat. solutions are not stable.)
35
752
341
IRON HTDROXmi (Ferric) Fe(OH)».
IRON H7DB0ZIDI
Solubility op Fbrric Hydroxide in Aq. Oxalic Acid SoLUTfON 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.
da of
Sat. Sol.
1.007
1. 015
1. 031
Gms. per loo Gms. Sat. SoL
FeA.
0.48
0.9s
1.86
CA.
0.61
1.23
2. 45
da of
Sat. Sol.
1. 040
1.050
1.064
Gms. per 100 Gms. Sat. Sol.
FeA.
2-33
2.98
362
CA.
310
3.8s
ntON NITRATE (Ferric) Fe(N0i),.9HA
Equilibrium in thb 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.
da of
Sat. Sol.
032
079
127
264
368
43S
498
1.496
Gms.
100 Gms.
iat. Sol.
SoUd Phase.
FeiOs. NA-
1.78 2.21 FeA-MNAffHiO
3-99 S-6i
S-79 9
7.22 12.31
9.70 16.60
12.48 22.70
14.62 28.13
15.40 29.52
15.22 30 . 50 F«A.3NAi8HiO
fi
II
II
II
II
II
(Hi of
Sat. Sol.
I
I
I
I
I
I
I
I
I
Gms. per 100 Gms.
Sat. Sol. •
Solid Phase.
•4S2
13.
•434
9-
•417
7-
.404
S-
.428
3-
■450
4-
•465
4-
.407
3-
.419
3-
FeA.
14
95
25
02
55
51
19
93
52
NA.
33 5 FeA.3NA.x8H,0
36.3
M
403
47-5
SS-a
47 . 2 Fe«(V4NA-iSW>*
49.6
M
M
M
* This salt was obtained accidentally and its preparation could not be repeated.
ntON NTTBATE (Ferrous) Fe(NOi),.6HiO.
Solubility
IN Water.
(Funk, 1900.)
r.
Gms.
Fe(NO^s
per 100
Gms.
Sol.
Mols.
Pe(NQ,)s
per 100
Mols.
HiO.
Solid Phase.
f.
Gms.
Fe(NQi)t
per 100
Gms.
Sol.
per 100
Mob
H.0
SoUdPhiM.
27
3S-66
5-54
Fe(N0k)s.9Hi0
-9
39-68
6.57
r^OJOMB^
21.5
19
36.10
36.56
5-64
576
II
H
0
18
41.53
45 14
7.10
8.23
M
15-5
37.17
591
M
24
60.5
46.51
62.50
8.70
16.67
M
Density of solution saturated at 18** >■ 1.497.
IRON OXALATE 342
mON OXALATE (Ferrous) FeC,04.2HsO.
Solubility in Water^t 25® Dbterminbd by the Conductivity Method.
(Sch&ler, 1905.)
The sat. solution contains 5.38.ior^ gm. mols. C1O4 per liter.
ntON OLBATE.
100 gms. glycerol (d - 1.114) dissolve 0.71 gm. iron oleate. (AaMlin. 1873.)
ntOH OXIDES, HYDROXIDE and SULPHIDE.
Solubility in Aqueous Sugar Solxttioiis.
(StcUe — Z. Vcr Zuckerind. so, 340. '00.)
% Suttr One Liter of Siigir Solutioos DiaaolTei MOIigniDf d: .
mSS^ F<^(OH)e at: Fe;0> at; Fe»04 at; Mitt
^«^ X7.4*. 45^ 7?. X7S*. 45*. X7.S". 45*. 75*. i7'f- 4^- 7^.
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 7.3
SO 2.3 1.9 3.4 0.8 I.I 14.5 10.3 14.5 9-9 19-8 9-1
ZEOH PHOSPHATE Fe^CPOJ,.
Thb Action op Water and op Aqueous Salt Solutions upom
Ferric Phosphate.
(Lacfaowics — Monatsh. Chem. 13, 357, '9a; Cameron and Hurst — J. Am. Chem. Soc. 26, 9SS, ^0
The experiments show that the ordinary precipitation methods for
the production of ferric phosphate give products which do not conform
to the formula Fe,(P04),. By digestmg 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 Fe,(P04)a varies from about
0.0026 gram removed by 5 cc. H,0 to 0.0182 gram removed by 800 cc.
H^ at the ordinary temperature.
Solubiltty 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 0°. The sat. sol. was analyzed for ammonia
and for residue obtained by evaporation.
per^ Gms. ^'j^'^il. Solid Phase. perTi) Gii, X%^£j9?h. ' Solid Phase.
Sat. Sol. »-'saTsS""- Sat. Sol. ^^^^^
0.884 5.606 Fet(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 13.92 viscous black deposit 18.83 O.445
7.91 14.61
SoLUBiLmr 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 sicid solutions of concentrations up to 5% for 4 months. Analyses
of tne sat. solutions and solid phases were made.
IC
M
II
d»oi
Gms. per xoo Gi
ms. Sat. Sol.
Solid Phase.
Sat. Sol.
1.0074
I. 0162
1.0244
I. 0310
1.0383
FeA.
0.0105
0.0205
0.0384
O.061I
0.0849
PA.
0.942
1.984
2.838
3 770
4.706
Solid Solution
((
tt
tt
M
tt
543 nton sDUAti
IRON SULFATE (Ferrous) FeS04.7HtO.
SOLUBIUTT OF FlSRROUS SULFATE IN WaTBR. (Fteenckd, 1907^
Gms. F^Qi Gms.
t*. - per too Solid Piiaae. t*. FeSOipwioo Solid PhMlb
GmsJ^ Gms. I^
—0.172 1. 0156 la 4S«l8 44.32 RSOb-yH^
—0.566 4.2852 " 50.21 48.60
— 1.063 8.7054 " 52 50.20
— 1. 511 12.713 " 54.03 52.07
— 1. 771 14. 511 " 56 . 56 tr. pt.54 . 58 " +PbSOi-|W)
— 1.82 Eutec 17.53 Ioe+FeSa,.7H/) 6o,OI 54-95 FeSC^Hrf)
O IS 65 FeSa,.7H/) 65 55-59 " umubk
+ 10 20.51 " 70.04 56.08
15-25 23.86 " 64.8tr,pt. ... FeS0,.4Hd0+FeS0,,H^
20.13 26.56 - 68.02 52.31 FeSCHrf)
25.02 29.60 " 77 45.90
30.03 32.93 « 80.41 43.58
35.07 36.87 « 85.02 40,46
40.05 40.20 « 90.13 37.27
di9.% of sat. sol. B I.219I (Grtenish and Smith, 1903)
Solubility of Ferrous Sulfate in Aq. Solutions of Lithium Sulfate at 30*.
AND Vice Versa. (SchiciiiemAkecs, 1910.)
Cms. per xoo Gms. Sat. Sol." «• i- j nt Gms. per xoo Gms. Sat. Sd. .... |>. ^
'— = ■ --- • SoLdPh«e. ' FeSO.. ' Li.SO.. ' ^.^dPfcu..
FeS04.7EW) 15.39 i6-8o LiiS04.IW)
" 12.68 18.31 "
" S-32 ".IS "
" 3-74 23.1s ;;
" o 25.1
" +Li,S04.HiO
Equilibrium in tsb System FerricIOxide, Sulfuric Acid and Water at 25^
(Cameron and Robiaaon, 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.)
Jn^ ^""Ig'^.^""- SoUd ^"■•gt'/gj.^"" S3lid
^■^'- FeA. " S0>.- ^*^- FeA. ' SO.. ' ^^•
1 . 001 o . 07 o . 1 1 Solid Solution 20 . 48 26.18 FeiQs.3S08. loHiO
I. on 0.62 0.94 " 19-77 28.93 "
1.045 2.03 2.65 " 10.87 31-35 Fe>B08.4SOgioH20
1. 131 6.18 7.40 " 0.16 35.96 "
1. 217 10.03 11.84 " 0.07 41.19 "
1.440 15.90 20.70 " 1.05 42.43 "
Solubility of Ferric Sulfate and of Ferrous Sulfate in Aq.
Solutions of Sulfuric Acid at 25®. (Wirth, xgxa-u.)
Results for Ferric Sulfate. Results for Ferrous Sulfate.
.- ,.^ , Gms. per xoo Gms. Sat. .. ,. , Gms. per xoo Gms. Sat.
Normahtyof SoK NoriMhtyof Sol. Solid Phase,
used Add. ' < * » used Acid. . » » i^uu a uw.
FeA - Fe,(S04)^ uaea /una. j.^ ^ ^^^^
FeS0«.
UiSO,.
24.87
0
24-45
4
21.15
5.58
18.79
II. 16
16.51
15-81
16. II
16.50
2.25 9.99 25.02 2.25 10 19-03 FeS04.7HsO
6.685 5.82 14.58 10.2 5.414 10.30 ''
19.84 0.02 0.05 12.46 3.816 7.26 FeSOi.HiO
15.15 2. II 4.015
19.84 0.08 0.1522
ntON SULFATE
344
Equilibrium in thb System Ferric Oxide-Sulfur Trioxide- Water at 25^
(Wirth and Bakke, 1914.)
(The mixtures were shaken for 3-4 weeks.)
Gms. per
100 Gms.
Gms. per
100 Gms.
Sat.
Sol.
SoUdPhiae.
Sat. 2
Sol.
SoKd Phase.
FcA.
SO*.
FcA.
SO,.
• • •
71 23
notdet.
14.49
31-45
unstable
0.24
56.84
u
15-71
31.88
M
353
« j
pxob. Fei(S04)a.H^«.9H|0
20.21
31-30
U
+Fei(S04),.H«SO«.3H40
9.39
31 -54
Fe,(SOJ,.H«SO4.8Hi0+
6.6s
32 IS
Fei(S04)«.HtSO«.8H<0
Fe,(S0,),.9H^
9-39
31 54
" +Fe(SOJ,.H,S04.3H40
11.06
29-43
Fe,(S04),.9H^
12 03
3151
Fe(S04)«.HtS0«^Tl<0
13-88
28.33
It
13 27
31 84
II
15-23
27.92
M
13-68
31 78
unstabla
16.07
27.98
M
Results are also given for the two forms of yellow ferric sulfate (a copiapite and
fi copiapite) also for ferric hydroxide and sulfate solutions.
It was found that a saturated solution of FeiCSOOt.HiSOi.SHiO in abs. alcohol
at 25^ contained 8 gms. FeiOi + 17.18 gms. S0| (Ratio, i : 4.235) per 100 gms. sat.
sol.
The yellow ferric sulfate Fes(S04)i.9HiO is less soluble in alcohol. After 4
weeks snaking at 25^, 100 gms. of the sat. solution in abs. alcohol contained 4.497
fms, FetOi and 6.77^ gms. SOt (Ratio, i : 3.006). Thus the alcoholic solution,
jUSt as the aqueous, is considerably more acid than the solid phase with which it
18 in equilibrium.
100 grams sat. solution in glycol contain 6 gms. FeSOi at ordinary temperature.
(de Coninck.)
ICO gms. anhydrous hydrazine dissolve i gm. ferrous sulfate at room temp.
with decomposition. (Welsh and Broderson, 1915.)
Solubility of Mixtures op Ferrous Sulphate PeS04.7H,0 and
Sodium Sulphate Na,S04.ioH20 in Water.
(Koppd — Z. physik. Chem. 52. 405, '05.)
s^<
100 Gms.
Gms. per
100 Gms.
t*.
lltioD.
HsO.
Solid Phase.
teSQ..
N«,S04.
'FCSO4.
NasS64.
0
14 54
4-93
18.06
6. II
FeS04.7HsO + NasSQ|.io^O
IS -5
17.76
II
.32
25-05
15-97
U M
21.8
16.37
IS
■32
24 -34
22.51
FeNa,(S04),.4BW>
24.92
16.21
IS
•13
23.62
22.04
M
35
16-35
14
.98
23-91
21.83
M
40
16.37
IS
.42
24.01
22.62
«
18.8
18.13
13
.8
26.63
20.28
FeNas(S04)i4H«0 + FeSO«.7H^
23
19.58
12
•S
28.82
18.4
M M
27
20.97
II
■3
30 -95
16.64
M M
31
22.91
9
•71
33-99
14.41
M m
35
23- 8s
9
.26
35-66
13-85
m m
40
26.32
7
8S
39 98
11.92
M <•
18.8
18.23
14,
83
27.23
22.16
FeNas(SQ|}94HsO + Na«SQiJoHiO
23
13-83
18.
04
20.31
26.48
M M
28
7.66
24,
41
11.28
35-94
M «
31
458
29.
50
6.95
44.75
U «•
35
4.04
30-
49
6.16
46.58
FeNaflSQi.4HsO + Na^Sa
40
4.10
30.
60
6.27
46.99
M w
345 ntON SULFATE
ntON Potassium SULFATE (Ferrous) FeSO4.KsSO4.6H1O.
Solubility in Water. (Tobicr, iSss)
M Gms. KtFe(S04)| ^ Gms. K«Fe(Sa)i
per xoo Cms. HtO> per zoo Cms. HfO.
o 19.6 35 41
10 24.5 40 45
14. S 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
70.1. 10"* mols. FeS = 0.00616 gm., determined by conductivity method.
(Weigd, 1906. 1907.)
Additional data for the solubility in water are given by Bruner and Zawadzki.
100 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.
ntON SULFONATES.
Solubility of Iron Phbnanthrenb Sulfonates in Water at 2o^
(Sandquist, 191a.) ^^ Anhydrous Salt
^^* per 100 Gms. I^.
Iron 2-Phenanthrene Monosulfonate 5HsO 0.044
" 3- " " 5H,0 0.20
" 10- " " 6H,0 0.16
IRON THIOCTANATE (Ferric) Fe(CNS),.3HtO.
Distribution between Water and Ether. (Hantach and Vagt. 1901.)
Results at 25^. Results at Several Temperatures.
Gm. Mols. Fe<CNS)i per liter. ^ Gm. Mols. Fe(CNS)i per Liter. ^
y ' "> "/• **• r~ * "N "
HiO Layer (c). Ether Layer (O- ^ HfO Layer (c). Ether Layer (cO- ^
0.0202 0.0108 1.87 o 0.0089 0.0167 0.532
O.OII9 0.0034 3.51 10 0.0127 0.0128 0.995
0.0066 0.00093 7.07 20 0.0165 0.0091 1. 814
0.0035 0.00025 13.95 30 0.0196 0.0059 3.303
35 0.0207 0.0048 4.32
Results for the efiect of HNOt upon the distribution at 25*^ are also given.
ITAGONIC ACm CH,:C(COOH)CH,COOH.
Data for the distribution of itaconic acid between water and etber at 25* are
given by Chandler, 1908.
KERATIN.
100 gms. HiO dissolve 8.71 ems. keratin at 20-25^ (Dehn, 19x7.)
100 gms. ac|. 50% pyridine dissolve 16 gms. keratin at 20-25**. **
Pyridine mixes with keratin in all proportions at 20-25^. "
JLKxrTUii Kr. Solubility in Water, (von Antiopoff, 1909-10.)
(Results in terms of coefficient of absorption as defined bv Bunsen, see p. 227, and
modified by Kuenen in respect to substituting mass for volume of water involved.)
t*. Aba. Coef. (First Series). Abe. Coef. (Second Series).
o 0.1249 0.1166
10 0.0965 0.0877
20 0.0788 0.0670
30 0.0762 0.0597
40 0.0740 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 ACm
346
LACTIC ACm («) CH,CHOHCCX)H.
Distribution Bbiwbbn Water and Ethbr.
(Pinnow, 191 s-)
Results at 15^
Results at 27.5^
Gm. Mob. Add per Liter:
1*
Gm. Mob. Add per Liter:
<•>.
faiOUyer(»).
Ether Layer («).
HgO Layer (»). Ether Layer («).
W
Z.98
0.215
9.19
I -354 0.130
10.42
I -351
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.OI18
12.27
0.0548
0.0046
11.88
F.-pt. data for mixtures of trichlorolactic add and dimethylpyrone aie given by
Kendall, 1914.
LACT08I (see sugars, pages 695-7).
LANTHANUM BBOBCATE La(BiO,),.9HA
100 gms. H|0 dissolve 28.5 gms. lanthanum bromate at 15^ (Maiignac)
LANTHANUM CIT&ATE 2(LaC,H<Or).7HsO.
100 gms. aq. citric solution containing 10 gms. citric add per 100 cc., dissolve
0.8 gm. La(C«Hi07) at 20^ (HotmSbeis, 19070
LANTHANUM CobaltiCTANIDI La,(CoC•N«)^9H|0.
100 gms. aq. 10% HCl {du » 1.05) dissolve 10.41 gms. salt at 25^.
(James ami Willand, 19x6.)
LANTHANUM QLTCGLATI La(CHA)i.
One liter H|0 dissolves 3.328 gms. La(C|H]Oi)i at 20^ Qantsdi ami Gcunkiaut, 1912-13.)
LANTHANUM lODATE La(IO,)i.
Scx^UBiLiTY IN Water and in Aq. Salt Solutions at 25^
(Harkins and Pearce, 19x6.)
1000 gms. HiO dissolve 0.6842 gm. La(IOs)i at 25^ dj^ sat. sol. - 0.99825.
~ Cone, of
Salt. Salt. MiUi-
NoonaL
La(NOk)i 2
S
xo
so
100
200.5a
0.0990
0.4957
0.9914
X.9828
0.0913
0.4560
0.9130
X.8260
3.6530
4.5326
6.7989
KlOk
NalOk
ti
It
it
€t
tt
«
Gms.
d«. of
Cone, of
Gmt.
tf.. of
UdOi),
Salt.
Salt,MiIli-
LidO,),
per Liter.
Sat. Sol.
per Liter.
Sat. Sol.
0.559s 0.99732
NaNOk
25
O.869OX
1.00250
0.5288 0.99807
«
so
0.99040
1.00385
0.5194 0.99859
i(
100
I. 1603
1.00742
0.5522 ]
[.00212
i(
200
1.385
X. 01 290
0.6214 ]
[.00661
It
400
X.636
X. 0242 2
0.7431 1
C 01533
tt
800
2.156
1.04677
0.6290 ]
[.00030
tt
MM
x6oo
2.859
X. 09005
0.5633 1
[.00027
(<
3200
3.030
I. 17243
0.4970 1
0.3738 3
[.00030
[.00031
La(N(X)..-
2NH4NO1
26.34
0.631
X.OOXX2
0.63538 1
[.00060
ti
52.68
0.674
1.00355
0.56466 ]
[.00059
ti
105.36
0.7S4
X.OO97I
0.5083s 3
[.00065
tt
158.04
0.816
X. 01608
0.39938 3
[.00065
tt
196.83
0.867
X. 02 183
0.19736 1
[.00069
(t
393.67
1.063
1.04343
0.13393 5
[.00083
tt
787.3s
1.364
X. 08286
0.09733 1
[.00130
tt
1574.70
1.923
X. 16652
According to Rimbach and Schubert (1909), one liter H^ dissolves 1.681 gms.
Li(IOs)i at 25^ determined chemically, and 1.871 gms. determined dectrolytically;
solid phase, 2La(IOi)t.3HiO.
LANTHANUM MALONATE La,(C|Hi04)s.5HsO.
100 gms. aq. Am. malonate sol. (10 gms. per 100 cc.) dissolve 0.2 gm. ) Lai(C|Hi04)t
[. malonic add sol. (20 gms. per loocc.) dissolve 0.6 gm. ) at 20^
100 gms. aq.
(Hohnbetg, X907O
347 LANTHANUM MOLYBDATl
LANTHANUM MOLYBDATE La,(Mo04)i.
One liter H|0 dissolves 0.0179 g™- Lat(Mo04)t at^25** and 0.0332 em. at 85*.
_ (Hitchcock, 1895.
LANTHANUM Ammonium NITBATE La(NOi)i.2NH4NOa.
100 gms. HiO dissolve 181.4 gms. La(NOj)j.2NH4NOj at 15*. (Holinbeig, 1907.)
LANTHANUMj Double . NITRATES.
Solubility of Lanthanum Double Nitrates in Conc. HNO«(({ifl » 1.325)
AT 16**. aaotach. 191a.)
^ , Gms. Hydnted Salt
Salt. Fonnala. Diaaolvedper
Lanthanum Magnesium Nitrate [La(NO|)«]sMgt.24HfO 6^.8
Nickel " '* Ni, " 80. ^
Cobalt " " Co, " — -
Zinc " " Zn, "
xoQ.a
124. z
Manganese " " Mn, " 193.1
LANTHANUM NITRATE La(NO.)s.
Solubility of Lanthanum Nitrate in Aqueous Solutions of Lanthanum
Oxalate at 25^ and Vice Versa. Games and WhittemoK, 19x3.)
Gms. per TOO
Gms. Sat. Sol.
La(NQi)v'
Solid Phase.
Gms. per 100
Gms. Sat. Sol.
Solid Phase.
LttCCfOJ,.
La,(C,04),.
U(NOk),. '
0
60.17
U(NQi),
not det.
not det.
I*i(CA)t.sH|0
0.67
59-91
II
332
42.27
La,(C^«)a.8H^
2.10
59 03
If
2.80
38-50
M
2.23 •
59 03
" +Lt.(Ci04)^3HiO
2.51
35-57
M
2.26
58.22
La«(C^«)t.5H«0
2.21
31.53
M
2.34
55 20
<i
•
2.01
28.63
M
2.47
52.74
M
1.46
22.15
M
2-59
49.84
U
1. 18
17.99
M
2.68
45-26
M
0.50
9.89
M
not det.
not det.
JMCfid^sBfi
0.28
5.06
«
LANTHANUM OXALATE La,(C,04)i.9HsO.
One liter water dissolves 0.00062 gm. Las(Cs04)i at 25^ determined by electroly-
tic method. (Rimbach and Schubert, 1909.)
100 gms. aq. 10.2% HNOt (d = 1.063) dissolve 0.80 gm. LasCCiOOi at I5^
(y. Scheele, 1899.)
100 gms. aq. 19.4% HNOt {d » 1.116) dissolve 2.69 gms. Lai(Cs04)i at I5^
(v. Scheek, 1899.)
Solubility of Lanthanum Oxalate in Aq. Solutions of Sulfuric
Acid at 25^ (Hauser and Wirth, 1908; Wirth, 1908; Wirth, x9xs.)
Normal- Gms. oer too Gms. Nonnal- Gms. per 100 Gms.
ityof Sat. Sol. Solid Phase. ity of Sat. Sol.
HfSO*. LaA - La,(CO«)^ HiSO«. La^ - La,(C,OJ,.
o.x 0.0208 0.0346 Lat(C204)t.9HiO 2 0.4417 0.7344 Lat(CiO«)s>9HtO
0.5 0.0979 0.1629 " 3.09 0.680 1. 1306 "
I 0.2383 0.3962 " 4.32 0.880 1.4630 "
1-5 0-319 0.5304 " 5.6 1.092 1. 8155 "
Solubility of Lanthanum Oxalate in Aq. Solutions of Oxalic Acid.
AT 25^. (Hauser and Wirtb, 1908.)
Normality of Aq. Gms. per 100 Gms. Sat. Sd. g^jy pj^^^
<>*»^Add. ' l^ Z Lt.(C04),.^
o . I unweighable Lat(Ci04)i*9HaO
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 adds.
100 cc. aq. 20% triethylamineoxalate dissolve approx. 0.032 gm. Lai(Cs04)t.
(Grant and James. 19x7.)
XiANTHANUK PH08FHATI 348
LANTHANUM Dimethyl PHOSPHATE Lai[(CH«),P04]<.4HsO.
100 gms. H]0 dissolve 103.7 Sms. Las[(CHi)iP04]« at 2$"*, (Mocgu and Jaiiwi||i9i40
LANTHANT7K SULFATE U>(S04)».9H>0.
Solubility in Water. (Muthmaim and Rsils, X898J
r.
Gnu. LatCSOJjper xoo Gms.
^ Gms-LatCSOf).
per 100 Gms.
Soludon. Water.
Solution.
Water. '
0
2-91 3
SO 1.47
I-S
14
2.53 2.6
75 0.9s
0.96
30
1.86 1.9
100 0.68
0.69
Solubility of Lanthanum Sulfate in Aq. Solutions of Ammoniuic
Sulfate, Potassium Sulfate and Sodium Sulfate. (Bane, 19x0, 19x1.)
In Aq. (NH4)sS04 at I8^ In Aq. KtSOi at I6.5^ In Aq. NatSOi at 18*.
Cms, per loo Gms. HjO.
<NH«)sS04. LaiCSOOi.
4.01 0.393
8.73
18.24
27.89
36.11
47-49
53.82
65.29
73.78
0.279
0.253
0.476*
0.277*
0.137
0.067
0.0117
0.0033
Solid
Phase.
1. 1. 2
((
(C
€i
«
2-S
'J
u
Gms. per xoo Gms. H^O.
K«SO«.
O
0.247
0.496
0.846
1.029
1. 156
La,(SO,),.
2.198
0.727
0.269
0.185
0.054
0.022
Solid
Phase.
1.0.9
1. 1.2
i-S
Gms. per loo Gms. HjO.
Na«SO«. Lat<S04)«.
O
0.39s
0.689
0.774
1.136
2.480
3.802
5 548
2.130
0.997
0.353
0.299
0.129
0.044
0.019
0.016
* M unstable equilibriiim.
Solid
Phase.
1.0.9
1. 1. 2
i(
a
U
tt
(NHO.
1.0.9 " Lai(S04)i.9HiO. 1.1.2 = Lat(SO4)i.X|SO4.2Hi0 (where X
K or Na). 2.5 = 2U,(S04)i.5(NH4)iS04, 1.5 =:.La,(S04)s.5^iS04.
S(X.UBiLiTY OF Lanthanum Sulfate in Aqueous Solutions of Sulfuric
Acid at 25**. (Wirth. 191a.)
Normality
of Aq.
Gms. per xoo Gms.
£t. Sol.
Solid
Phase.
Normality
of Aq.
H,S04.
Gms. per 100 Gms.
Sat. Sol.
SoOd
Phase.
H^4. .
La,0,= La,(S04),.
LaA - La,(S04),.
Water
1.43 2.483
UtCSOdt.9B^
4.321
I. II 1.927
Lat(S04),.9HiO
0.505
1.69 2.934
It
6.685
0.531 0.9217
u
1. 10
1.796 3. 118
M
9.68
0.266 0.4617
«
2.16
I. 818 3.156
U
12.60
0.214 0.371
M
3-39
1.42 2.465
U
15.15
0.177 0.307
«
Data for the solubility of lanthanum sulfate in aq. HtS04 in presence of solid
oxalic acid at 25^ are given by Wirth, 1908.
LANTHANUM SULFONATES.
Solubility of Each in Water.
Sulfonate.
TAiithannm Benzene Siilfonate
" ffi Nitrobenzene Sulfonate
" ffi Chlorbenzene Sulfonate
" ffi Brombenzene "
Formobu
LalCASQ,l,.9H/)
La[CcH4NQ|S0k]|.6H^
La[CACI.S0.]..9H«0
La[ciH|Br.S0k]«.9Hi0
Gms.
Anhvdrous
Suliooatc Authority,
per 100
Gms. H^.
63.1 (Holmbeig, 1907*)
16
13. 1
12.9 **
" (6) Chloro (3) Nitrobenzene (i) JSulfo- j UICAC1(NQ,)S0J,.8H|0 24 . $
" (i)
Bromo (4) Nitrobenzene (2) ) nate ) La[QH»BrN0^SOk]|.8HiO $ (Katz ft James, '13.)
" a Naphthalene Sulfonate La[CioHTSOk]i.6H^ 5 . 2 (Hohnbexg, 1907.)
" 1.5 Nitronaphchalene Sulfonate LaicMH«(NQi)SOftU-6H^ 0.55
" 1.6 " " " .9H^ 0.21
M
l<
1.7
it
u
.9fliO X.X
349 LAHTHANUM TABTRAtl
LANTHANUM TABTRATE La,(C«H/).),.9HsO.
One liter HiO dissolves 0.059 gm. Lat(CiOA)t at 2$"* (solid phase LatCCiH^Oi)*-
3H1O). Determined by electrolytic method. (RimUch ud Sdmbeit, 1909^
Solubility of Lanthanum Tartrate in Aq. Tartaric Acid and Ammonium
Tartrate Sch^utions at 20^.
(Hohabefg, 1907.)
In Aq. Tartaric Acid. _ In Aq. Ammonium Tartrate.
Gms. Tartaric Add per Giiis.La«(Q04Qi)«Der ~ Gma. Am. Tutxate per Gms. Lat<C|HA}s per
100 cc Solvent. xoo Gms. SaL Sol. zoo oc. Sohreat. zoo Gmk Sat. SoL
20 0.6 ID 0.2
40 1.2 20 0.6
LANTHANUM TUNQSTATE LatOVOi)..
One liter H^ dissolves 0.0117 gm. LasCWOOi at 27^ and 0.0236 at 65^
u (Hitchcock, zSqsO
LAUBIC ACm CisHttCOGH.
SOLUBILITT IN AlCOEGLS.
(Tunofeiew, 1894.)
Methyl Alcohol o 14.8 Propyl Alcohol o 21.5
21 58.6 " 21 52. 6
Ethyl Alcohol o 20.5 Isobutvl Alcohol o 18.4
" 21 57.3 ^* 21 49.7
LEAD Pb.
An extensive investigation of the solubility of lead in the water pasang through
lead pipes is described by Paul, Ohlmuller, Heise and Auerbach, 1906. ^ The
solubility is increased by oxygen, COi, sulfates and perhaps other salts; it is de-
creased by hydrocarbonates.
SOLUBIHTY OF LeAD IN LiQUID AmMONIA-SODIUM SOLUTIONS AT —33*.
(Smith, F. H., 1917.)
Gm. Atoms Sodium Gm. Atoms Pb Gm. Atoms Na Gm. Atoms Pb
r Gm. per Liter of Liquid Dissolved oer Gm.
Ammonia. Atom Na.
0.13 2.17
0.14 2.12
0-33 I 83
0.34 1.73
LEAD ACETATE Pb(C,HsOt)s.3HA
100 gms. HsO dissolve 55.04 gms. Pb(CiHsOi)s at 25^ Gackaon, z9z4-)
Equilibrium in the System Lead Oxide, Acetic Acid, Water at 25^
(Sakabe, 19x4-}
Gms. Der 100 Gms. Sat. Sol. „ ,. . « Gms. per zoo Gms. Sat. Sol. _ ,. . ^.
' PbO. CH.COOH.- ^^^^^^ ' pbo. ■CH.COGH.- SobdPhase.
4.18 21.53 Pb(CiHA)»3H^ ^ -- ^ ^fi (CHA)(HO)Pb+
3.80 16.78 « '^^ ' (CiHW,Pb.2(H0)«Pb
3,16 13.07 " 5.20 5.61 ((^|HA)iPb.a(HO)tPb
2.64 5.49 « 3.78 4.17
3-34 5-36 « 2.89 2.51
438 730 " 1-45 I 03
5.18 7 . 92 " +(CHA)(HO)Pb 1 . 05 0 . 54 PbO
5.59 7.72 (CHA)(HO)Pb 1.07 0.48
6.51 7.79 " I 0.20 «
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.
Liter ot Liqwd
Ammonia.
Dissolved De
AtomNi
0.078
1-95
0.093
2.20
0.094
2.03
O.IIO
2.24
0.12
1.78
II
II
LIAD ACETATE 550
Equilibrium in thb System Lead Acetate, Lead Oxide, Water at 25^
(Jackson, 19x4.)
. JyOf
Gms-perioo
Gms. Sat. Sol.
Solid
Phase.
Sat. Sol. '
vms. per xoo Gms. Sat. Sd
PbO. Pb(CaiA)s.
• Solid
Sat. Sol.
PbO.
Pb(CaiA)«.
Phase.
1.326
— 0.27*
35-19
1-3
2.280
24.74
49-21 3
.1.3+1.24
1-334
'+O.IO
35-60
((
2.048
23-59
43.17
1.2.4
I 367
1. 01
37-14
((
I -951
22.78
40.78
tt
1.422
3.38
38.93
<(
X.657
19.63
31-40
tt
MM
I 531
6.01
41.95
tt
1.599
X8.73
29.63
tt
1.658
9-47
44-71
t(
1.382
14.62
20.96
tt
• • •
14.22
47-88
((
1.348
13-41
19-65
tt
1.852
14.44
47.92
it
1.229
10.66
12.99
tt
• • •
15.89
48.951.
3+3-1
•3 I -157
8.47
8.64
tt
MM
1.930
15-90
48.42
3-I-3
1. 119
7.87
5-27
tt
1.942
16.25
48.85
U
1. 117
7.79
5-25
tt
1.956
16.65
49.04
tt
• • •
7.17
4.17
Pb(OH),
2.024
18.83
48.71
t<
1. 100
6.84
4-31
tt
2. 161
22.23
48.52
(t
1 095
6.54
4-25
tt
2.193
22.94
48.96
U
1. 08s
5-91
3-82
mm
• • •
23.28
49-14
ii
I -075
5.29
3 40
tt
mm
2.220
23-53
49.01
n
• • •
0.20
O.II
tt
* In this case the acidity is expressed in tetxns of PbO.
i.j=Pb(C,H,0,),.3HA 3.i.3=3Pb(C,Hrf),)i.Pb0.3HA 1.2.4 =.Pb(CHrf),V
2Pb0.4HiO.
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 davs. 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 neutrali^d 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, X909.)
Gms. per xoo Gms. Sat. Sol.
cScOOK! " (CH,COO).Pk ^^ ^^^
o 35.9 (CH,COO)2Pb.3HiO
13.87 38.05
15.40 36.90
tt
(t
Solubility of Lead Acetate in Aqueous Solutions of Ethyl Alcohcm^ at 25^.
(SeideU, xgxo.)
Wt.% j^ Gms. Wt.% j^ Gms.
CHjpH ^ (CH,CW.Pb Solid Phase. ^^ Ikt (CJH^.Pb SoUd Ph««.
"* Q^ per xoo Gms. "^j*-** -^"m*. m ^^- per xoo Gms. »3wuu i^umc.
Solvent. ^- Sat. Sol. Solvent. ^'- ^at. Sol.
o 1.343 36. S (CiHA)iPb.3H|0 70 0.9SS 12.4 (CaHjQi)iPb.3HiO
10 1.27s 32.3 " 80 0.907 9.4 "
20 1.21$ 28.6 " 81 0.905 9 '*
30 1. 157 2$ " 8s 0.8SS 4 (CjHjQi)iPb
40 i.ios 21.9 " 90 0.826 1.6 "
SO 1.05s 18.7 " 9S 0.806 0.6 **
60 1.002 1S.6 " 100 0.790 0.4 "
100 gms. 95 % formic acid dissolve o.99(?) ™. Pb(CiH|Oj)s at 10.8*. (Aschan. xgxj.)
100 gms. anhydrous lanolin (m. pt.46*') dissolve i.igm. Pb(CiH/>3^at45®. (Klose/o?.)
100 gms. glycerol dissolve about 20 gms. Pb(CsHaOt)t at 15^. (Ossendowski. X907.)
LIAD ARSENATE PbHAs04.
Two gm. portions of amorphous dilead arsenate were agitated at 32^ with 90 to
180 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 AssOi varying
from 1.956 to 1.429 gms. per liter. (McDonnell and Smith, 1916O
351
LEAD BINZOATI
LKAD BINZOATE Pb(C7HiOs)t.HsO.
Solubility in Water.
(PajetU, 1906.)
f. x8'. 40.6'. 49'.
Gms. Pb(C7H602)s per 100 gms. sat. sol. o . 149 o . 249 o . 3 10
LKAD BORATE Pb(BOt)2.HsO.
100 cc. anhydrous hydrazine dissolve about 2 gms.,Pb(BOs)t at room temp.
(Webh and Brodexaoii, 1915.)
LEAD BBOMATE Pb(BrC)i.H,0.
100 gms. water dissolve 1.32 gms. Pb(BrOi)t at 19.04^.
(Ri
ammebbecg, 1841; BOttser, x90)3.)
LEAD BBOMIDE PbBr,.
Solubility in Water.
(Liclity — J. Am. Chem. See. 25, 474, '03.)
t\
Density
of Solutions,
H^ at oo.
Gms. PbBri per xoo
MflUgnrnMo
cc. Solutioa.
b. PfaBr^ per n
cc. Solutkm.
Gms. H«0.
Gms.B/}.'
0
1.0043
0.4SS4
0.4554
1.242
1.242
IS
I 0053
0.7285
0.7305
1.987
1.989
as
I. 0061
0.9701
0.9744
2.646
2.655
3S
1.0060
1. 3124
1 .3220
3577
3 603
45
I 0059
I 7259
1-7457
4 705
4.760
S5
1.0046
2 . 1024
2.1376
5-731
5 Say
6S
1.0028
2.516
2-574
6.859
7.016
80
1. 0000
3-235
3-343
8.819
9-"3
95
0.9995
4.1767
4 3613
11.386
11.890
zoo
• • •
4 550
4.751
12.40
12.94
Solubility op Lead Bromide in Aqueous Hydrobromic Acid
AT 10®.
100 grams H,0 containing 72.0 grams HBr dissolve 55.0 grams
PbBr, per 100 gms. solvent, and solution has Sp. Gr. 2.06.
(Ditte — CompC. rend 92, 719. '8x^
Solubility of Lead Bromide in Pyridine.
(Heise, 19x2.)
t".
Gms. PbBrt per
xoo Gms. Pyridine.
SoUd Phase.
r.
Gms. PbBri per
xoo Gtta, Pyridine
SoUd Phase.
9
-26
1.02
PbBr,.3C|H|N
45
0.661
PbBrs.ar4H,N
— 10
0.89
11
64
0.800
11
- 5
0.84
M
77
0.969
«
0
0.80
M
95
1-33
M
+13
0.661
M
100
1.44
M
19 tr.
pt.
• • •
" H-PhB^iriHiN
loS
1.56
M
26
0.58.^
PbB4.3C|H,N
•
Freezing-point Data (Solubility, see footnote, p. i) are gfven for
Following Mixtures of Lead Bromide and Other Compounds.
Lead Bromide + Lead Chloride
+ Lead Iodide
" " -j- Lead Fluoride
+ Lead Oxide
** ** -|- Mercuric Bromide
" " + Silver Bromide
(MSnkemeyer, X906.)
(i
(Sandonnini, x9xx.)
(Sandonnini, X9X4.)
(Sandonnini, 19x9, 19x4.)
(Matthes,- X9xx.)
UAD BBOMIDl 352
LIAD Dicydohexyl DiBROMIDl (C«Hti),PbBrt.
LKAD Dicydohexyl DiCHLORIDE (C«Hii),PbClt.
Solubility of Each in Several Solvents at 22.5^.
(Gilittner, i9X4')
Grams per zoo Grams Solvent.
Solvent. r" ^ "^
(C|Hu)iPbBr,. (C,Hu)tPbCV.
Benzene 0.014 0.016
Carbon Tetrachloride o . 004 o . 004
Chloroform 0.078 0.083
Alcohol + Pyridine (1:1) 2 . 560 2 . 904
Similar results are also given for lead tetracydohexyl, Pb(C«Hii)4, lead tetra-
phenyl, Pb(C«Hi)4, and lead diphenyldicydohexyl, Pb(C«Hi)i(C6Hii)2.
Gms. per xoo Gms. Solvent.
%
Solvent. / *
Pb(C^„)4. Pb(CH,)4. Pb(CH«),(C,Hu)i.
Alcohol o.oio 0.020 0.324
Benzene 1.068 1145 2.298
Carbon Tetrachloride 0.244 0.303 0.845
Ethyl Acetate o . 030 o . 1 23 0.231
UAD CAPBOATE, CAPBYLATE, CAPRATE, etc.
Solubility of Each in Ether and in Petroleum Ether.
(Neave, X9X3.) i
Solubility in Ethyl Ether. Solubility in Pet. Ether.
Gms. Salt per xoo cc. Sat. Sol. Gms. Salt per 100 oc. Sat. SoL
Lead Salt. Melting point. / ^ \ / ^ s
At 30*. At B. pt. of Sat. Sol. At 90*. At B. pt. of Sat. SoL
Pb Caproate 73-74 ... 1364 ... 0.0608
" Heptylate 90.5-91.5 0.2397 1490 0.020 0.0528
" Caprylate 83.5^4.5 0.0938 0.546 practically insol. 0.0384
" Nonylate 94-95 0.1115 0.2404 " 0.0450
" Caprate 100 0.0290 0.4285 " 0.0170
" Myristate 107 practically insol. 0.0555 " 0.0210
" Laiirate 103-104 " 0.0205 " practically insoL
" Pabnitate 112 " 0.0261
" Stearate 125 " practically insol. " 0.0170
The ethyl ether was distilled over sodium. Petroleum ether distilling between
40^-60*^ was us^. The solutions were stirred constantly at 20^ A definite volume
of the sat. solution was evaporated to dryness and residue weighed in each case.
LKAD CARBONATE PbCO,.
Solubility in Water by Electrical CoNDUcnvrrY Method.
(Kohlrausch and Rose, 1893; Bdttger, X903.)
I liter of water dissolves o.ooii —0.0017 gni. PbCOi at 20'.
Solubility op Lead Carbonate (Neutral) in Aqueous Solutions of
Carbon Dioxide at 18®.
(Pleissner, X907.)
Millimols per Liter. Milligruns per Liter.
CO,.
PbCO,.
CO,.
PbCQ,.
0
0.008
0
1.7s
0.064
0.029
2.8
6
0.123
0.034
54
7
0.328
0.040
14.4
8.2
0.592
0.048
26
9.9
0.988
0.053
435
10.9
2.40
0.076
106
15.4
A determination of the solubility of basic lead carbonate in water gave 1.6 tag,
Plh(CC^)t(OH)s per liter » 1.3 tag. Pb or 0.006 millimol Pb.
353 UAD CARBONATE
Data for equilibrium in the system composed of K2CO1 + PbCOi + KsCr04
+ PbCrOi 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, 191 1.
LEAD CHLORATE Pb(C10s)s.HA
100 grams HsO dissolve 15 1.3 gms. Pb(C10i)t, or 100 gms. sat. solution con-
tain 60.2 gms. Pb(C10i)i at 18*". Density of solution, 1.947. (Myllus and Funk, z897-)
100 gms. H^ dissolve 440 gms. Pb(ClOa)] at i8^ dit => 1.63. (Carlson, 19x0.)
LEAD CHLORIDE PbCb.
Solubility in Water. CLkhty; see abo Fonnanek, S887; Bdl» X867; Ditte, x88i0
Density Gms. PbCla per 100 MilUgram Mols. PbOs per too
HsO at o^. <^* Solution. Gms. HsO. cc. Solution. Grams HsO.
o 1.0066 0.6728 0.6728 2.421 2.421
IS 1.0069 0.9070 0.9090 3-265 3.272
25 1.0072 1.0786 1.0842 3.882 3903
35 1.0060 1.3150 1-3244 4-733 4767
4S 1.0042 1.5498 1-5673 5-579 5-^44
55 1.0020 I. 8019 1.8263 6.486 6.573
65 0.9993 2.0810 2.1265 7.490 7-651
80 0.9947 2. 5420 2.6224 9-150 9-439
95 0.9894 3-0358 3 1654 10.926 11.394
100 .. 3.208 3-342 II. 52 12.01
SOLUBILITT OF LEAD ChLORIDB IN AqUBOUS SOLUTIONS OP ACBTIC AciD
AT 25*. (Hfll. 1917.)
Normality Dissolved PbClt. Normality Dissolved PbCU.
«* Acetic "Gms! Equiv. ' ofAatic ''cms! ' Equiv. '
Add. per Liter. per Liter. Aad. per Liter. per liter.
o 10.77 0.07753 0.465 10.27 0.07392
Gms.
Equiv.
per Liter.
per Liter.
10.77
0.07753
10.82
0.07782
10.85
0.07717
10.70
0.07703
0.05 10.82 0.07782 0.929 9.45 0.06803
o.io 10.85 0.07717 1.845 7.90 0.05686
0.20 10.70 0.07703 3.680 5.26 0.0^788
SOLUBILITT OF LeAD ChLORIDE IN AqUEOUS AmMONIUM ChLORIDE AT 22^.
(Br5nsted, 19x1.)
Gm. Equivalents per Liter. _ ,. . ^, Gm. Equivalents per Liter. „ ..^ «,
' NH.C1. " PbCW. - SobdPhase. .^^^ ' PbCl,. ^ Sobd Phase.
O 0.0749 PbO, 0.8 0.0087 NH«a.aPbai
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.2pbCIi 6 0.0473
0.55 0.0123 NH«aaPbCI, 7.29 0.0898 " +NH«a
0.65 0.0105 " 7.29 o NH«a
For additional results at 25.2® see von Ende, 1901.
Solubility of Lead Chloride in Aqueous Solutions of Hydrochloric
AaD.
Results at I8^
(Pleissner, 1907.)
Results at 25.2**. (von Ende, 190X.)
Normality
Gms. PbOt
Normality
Millimols Normality MUUmoIi
ofHQ.
per Liter.
of HCl.
PbOs per Liter, of HQ. Pbdt per Lit«r.
0
9.34
0
38.8 1.026 4.41
O.OOOI
9.305
0.0045
37.35 2.051 5.18
0.0002
9.300
O.O151
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 75 65.86
0.0102
8.504
0.5142
5.37 12.05 164.30
LEAD GHLOBIDl
354
Solubility of Lbad Chloride in Aqueous Solutions op Hydro*
CHLORIC Acid.
(At 0^, Eogd — Ann. cUm.plm. [6] i% ^59, '89; at a^, Nojres — Z.pbyA, Chem. 0^625, 'pa; at diflo'
ent tempentnrest Ditte — Compt. rend. 92, 7x8» "Sz; see alio BeU — J. Chem. Sob. ax» 350, '68.)
Gffli.Ha
Gms. FbQi per
literal:
Gma. HCl
per 100
Gms. HsO.
Gms. PbGs
o*. «>•.
per 100 Gms. Solat
40*. sf-
ion at:
L&er.
o».
»f:
8o».
0
5-83
10.79
0
8.0
II. 8
17.0
21.0
31 0
OS
4 S
9.0
100
I. a
1.4
3-2
55
12.0
Z.O
3-6
7.6
ISO
i-S
2.0
5-0
75
16.0
a.o
3.3
6.0
aoo
3 5
50
8.2
"•7
21-5
30
1.6
S-o
250
6.5
8.0
13 0
l6.3
28.5
6
1.4
31
300
10.7
"5
175
33.0
35 -o
XO
I. a
1.8
400
ai.s
24.0
• • •
• • •
• • •
100
I. a
300
S-2
350
10.5
300
17s
'
400
40.0
Solubility op Lead Chloride in Aqueous Salt Solutions
AT 25^.
(Nojea; in HgOs solutions at so^ Fonnanek — Chcm. Centralb. sto* ^7.)
In Aqueous Solutions of:
Hd Kd Mga» CaCl» MnCli In CdCI^
and ZnQi Gram EauiTalents
per Liter ot;
Sir Pbai.
0.0 00777
0.05 0.050
o.io 0035
0.20 0.02Z
GramEkimy.
per Ijtcr.
CdCla. pEat.
0.00 0.0777
0.05 0.0601
O.IO 0.0481
0.20 0.03SS
In HsOs
Gram Eqiuv.
per Liter.
'H«ai. PbQi.
0.0 0.0777
O.I 0.0992
toPWO^
Gram Eqmv.
per liter.
l*b(NOa)s. Pbc5.
0.0
0.2
0.0777
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
per
Liter.
Grams PbCls per liter in Aqiieoos Solutions of:
0
10.79
I
8.5
9
6.5
3
5. a
4
4.3
6
3«
8
as
10
a.r
14
• • •
30
• • •
40
• • •
HQ. KQ.
10.79
9.3
8. a
7. a
6.5
5-3
4-5
3-9
31
• • .
a • •
MgQi. CaQi. MnQi. ZnQs.
10.79 10.79 zo
10.79
7.7
6.5
5-7
5 a
4.4
8.7
7.6
6.7
6.0
4.8
3-9
3-3
1.1
7-3
6.3
50
4.1
3
a,.
CdCls.
10.79
HgOs. Pb(NOk)s
.79
10-7900 9Zi(F) 10.79
10. a
II. 0
9.0 10 .0
9-7
II. 4
10. 0 10 .85
2!
II. 7
10.3 10.87
8.6
la.o
10.5 10.90
7-7
ia.7
II. 0 zo-95
7.0
13-3
II. 6 11.00
6.3
14.0
la.a IZ.05
•0
5-4
...
13. a II. 15
4.7
...
14.8 II. ao
...
...
19.0 11.70
355
^JIAD CHLoams
SOLUBILITT OF LRAD ChLORIDB IN AqUEOUS SOLUTIONS OP LeAD NiTRATB AT 25*.
Results by Harkinsy 191 1. Results by Armstrong and Eyre, 19 13.
Cms. per Liter Sat. Sol.
Pb(NO0,.
O
8.28
16.56
33.12
PbCl^
10.81
10.67
10.65
10.84
11.57
dL. of Sat.
*Sol.
1.0069
1.0095
I. 0139
I. 0210
Aq. Pb(NQOi
Sol., Gms. per
zooo Gms. afi.
331
6.62
82.80
Scx^UBiLiTY OP Lead Chloridb in Aqueous Solutions of Potassiuit
Chloride at 25^^ (von Ende, xgozO
Cms. PbQs per
1000 Gms.
Sat. Sol.
10.89
10.96
10.53
II. 15
12.95
Normality
ofKCl.
O
O.OOI
0.0025
0.0049
0.0099
0.0200
0.0599
Gm. Equiv. Pbdt
per Liter.
0.07760
0.07664
0.07570
0.07404
0.07056
0.06432
0.04524
Nofrmality
of KG.
0.0999
0.5006
0.7018
0.9991
I . 5018
2.0024
3 0036
Gm. Equiv. Pbd
per liter.
0.02380
0.01480
0.01476
0.00980
0.00996
O.OIII2 .
0.01948
Solubility of Lead Chloride in Aqueous Solutions of Potassium
Chloride at 20^. (Brsnsted, 19x3.)
Gm. EqoiyaleDts per
xooo Gms. ScrftttioD.
Solid Phaae.
Gm. EquivaleBts per
zooo Gms. Solution.
i<
M
M
KQ. PbO,.
0.195 0.01900 PbOt
0.299 0.01452
0.375 0.01324
0.483 0.01236
0.510 0.0125
0.575 0.01068
0.639 0.00954
0.930 0.00770
1.224 0.00736
1.575 0.00786
1.884 0.00894
" +aPbCI^Ka
aPbOiXa
u
u
u
KQ.
2.10
2.20
2.29
2.36
2.45
2.66
2.77
2.91
3 05
StlidPhaae.
sPbC^Xa
PbCl,.
0.01022
0.01060
O.OI184 -^
0 . 01300 aPbClfKa+PbClfKCLiH^
II
M
0.01308
0.01396
0.01476
0.01550
0.01656
0.01780
Pbda-KCLiH^
M
U
M
M
+Ka
318
4.57* 0.0280*
*M Gm. equivalents per xooo Gms. H^.
^ Data for the solubility of lead chloride in aqueous KCl and aqueous NaCl are
given by Demassieux, 1914.
Solubility of Lead Chloride in Aqueous Solutions of Alcohol and of
MannITOL at 25^ (Kemot and Pomilio, X9XS.)
Results for Aqueous Ethyl Alcohol. Results for Aqueous Mannitol.
Gms. per Liter Solution.
Gms. per Liter Solution.
CAGE.
Pbd.:
(CH«0H)s(CH0H)«.
Pbdt.
0
10 -75
0
10.75
5.75
10.16
2.84
10.42
II. 51
9 36
5.69
10.67
23.02
9.14
11.38
10.64
46.05
8.25
22.76
10.91
92.10
7.12
45 53
II. 16
184.20
4.76
91.06
11.29
SOLUBILITT OF LeAD ChLORIDE IN GLYCEROL. (Presse, 1874.)
I part glycerol + 7 parts HiO dissolve 0.91 per cent PbClj.
I part glycerol -j- 3 parts HiO dissolve 1.04 per cent PbClj.
I part glycerol + i part HjO dissolves 1.32 per cent PbClj.
Pore glycerol dissolves 2 per cent PbCli.
LEAD CHLORIDE
356
Solubility of Lead Chloride in Aqueous Solutions of Several
Compounds at 25®. (Annstronc and Eyre, 19x3)
Aqaeoiis
Solution ot:
Water alone
Glycol
Acetaldehyde
it
Paraldehyde
Gm5.Cmpd.^™f^
___ .,«_x per xooo
xooo
ms.HA
O
62.04
II. 01
33 03
II. 01
33 02
J>er I
ms. Sat.
Sol.
10.89
10.7s
10.90
10.54
9.82
10.50
9.96
Aqueous
Solution of:
Ethyl Alcohol
Glycerol
Propyl Alcohol
Methyl Acetanilide
Hydrochloric Acid
Cms. Cmpd. ^^,^
ms. Sat.
Sol.
cSs.ao. ^
II. 51
23.01
1501
60.06
29.82
9.12
18.23
10.43
10.98
10.08
9-37
10.25
4.23
360
100 cC anhydrous hydrazine dissolve 3 gms. PbCls at ord. temp, with decom-
position. (Welsh and Broderson, 1915.)
Solubility of Lead Chloride in PyrIdine. (Heise, 19x2.)
Gms. Pbdi
t*. per zoo Gms.
Psrridine.
0.893
1.07
t".
Gms-Pbdi
per 100 Gms.
Pyridine.
— 20
O
+ 22
44
65
0.303
0.364
0.4S9
0.559
0.758
Solid Phase.
PbCl,.2C5H6N
«
u
u
76
90
94
102
Sdid Phase.
PbCl,.2C6H6N
«
1. 12
I-3I
Freezing-point Data (Solubility, see footnote, p. i) are given for
THE Following Mixtures of Lead Chloride and Other Compounds.
Lead Chloride + Lead Fluoride
-j- Lead Iodide
-j- Lead Oxide
-j- Lead Sulfide
-j- Lithium Chloride
tt
11
41
14
<l
If
14
If
If
If
II
If
ff
II
II
II
II
ff
ff
ff
ff
ff
ff
ft
If
ff
ff
(Sandonnini, 1911.)
(Monkemeyer, 1906.)
(Ruer, 1906.)
(Truthe, 19x9.)
(Tries, 19x4.)
+ Magnesium Chloride (Menge, 19x1.)
+ Manganese Chloride (Sandonnini, x9xx, 1914.)
+ Potassium Chloride (Tries, 1914; Lorenz and Ruckstuhl, 1906.)
+ Rubidium Chloride "
-j- Silver Chloride
-|- Strontium Chloride
-j- Sodium Chloride
-j- Thallium Chloride
-j- Tin Chloride
(Matthes, 19x1; Tries, 1914.)
(Sandonnini, X9xi, 19x4.)
(Tries, X9X4.)
(Korrenx, X9X4; Sandonnini, 19x5.)
(Hermann, x9xx; Sandonnini, x9xx, X9Z4O
(Herrmann, 19x1.)
+ Zinc Chloride
LEAD CHLORIDE (Basic).
Solubility of Basic Lead Chlorides in Water at 18''. (Pidssner. X907.)
Onnpound
Formula.
Gms. per Liter Sat. Aq.
Solution.
Pb
0.079
0.021
PbSalt.
0.099
0.025
i Basic Lead Chloride PbClj.PbO.H2O
i " " " PbCli.3PbO.H,0
LEAD FluoroCHLOamE PbFCl.
Solubility of Lead Fluorochloride in Water and in Aqueous Solutions.
(Staric, X9XX.)
Solubility in Aq. Solutions at 25**.
Gms. PbFCl A^ c^i..*:— Gms. PhFO
Solubility in Water.
Gms. PbFCl
t*. , per xoo Gms.
H,0.
Aq. Solution wi». rurv.i Aq. Solution _
®*- ^t.Sol. °*- Sat.SoL
O
18
100
0.02II
0.0325
0.0370
O.IO81
0.00996 n PbCls 0.0030 0.0535 »HC1 0.0758
0.0195 n " 0.0008 o.io69n " 0.1006
0.0392 n " 0.0005 0.0518 n CHiCGOH 0.0512
0.1055 n " 0.0561
357 UAD CHBOHUTI
U&D OHBOMATK PbCtOt.
SoLUBiLiTV OF Lead Cbroiutb in Watkk.
„ Mob. pbCiO. Gn».PbCK). Utthod. AaU»rit*.
'■ per Liter. po Liter. ^ ...
iS 3.0.10"^ O.OOOIO Solution equilibrium (B«ck uid StigmtlUer, igtoj
I^-IO"' 0.00004. " " (AuethKh lad Pic±.)
18 3.2.10"' O.OOOIO Conductivity tKohlnuseh, 190S.)
aO 2.1. lO"' 0.00007 Radio Indicators (v. Oeven tad Room, rgijj
Solubility i
1 Aq. Hd.
Mmi(™i.Pbpoioo«.s
It. Sol. at:
t'S6
4-96
S7-. ■
7.40
8.15
10.06
IS.40
13 56
17-38
27.30
22.14
27.78
4360
33-30
43.60
68
46.60
61.06
97.20
lOlubility in
Aq.HN0.att8
NomuJityoI
HilliruuPbpec
HNO^
i«.<cSid.SaL
O.I
a. 67
0.3
4
70
0-3
6
46
0-4
8
31
o-S
10
31
0.6
13
39
Results are also given for the solubility of mixture* of lead chromate and
lead sulfate in aqueous hydrochlocic acid at 35° and 37*,
SOLDBILITY OP LEAD ChROMATB IN AqUSOUS PoIASSIUU HYDROXIDE ScS.Un0NS.
(I^dud ud Le^etre, tlgr.)
t*. OnmaKOHpariBaw. OmniPbCrGkpef icosc-
15 2308 I 19
60 3 -308 1 .63
80 3 .308 3 -61
I03 3 .308 3 .85
LSAD OITRATI Pb(C^,0,)..H,0.
Solubility in Water and in Alcohol.
100 gms. H,0 dissolve 0.04301 gm. Pb(C,H,0,),.H,0 at iS", and
O.0S344 gm. at 35°.
100 gms. alcohol (93%) dissolve 0.0156 gm. Pb(CJI,0,)^H,0 at
18°. and 0.0167 gm. at 15°. (PutbelluidHainn— ArcliiT.Plium.Mi. 413. '03J
LIAO D017BLI CTAHIDKS.
SOLUBILITT IN WATER.
(Sdtnlef— Sliber.Akul.WlM. Wien,7C>3(». 'n3
Ftmiuk.
Gim. RT too
DooUeSih.
Lead Cobalticyanide
Lead Cobalticyanide
Lead Potassium Cobalticyanide
Lead Cobalticyanide Nitrate
Lead FertJcyatiide Nitrate
Lead Potassium Ferricyanide
LEAD rLUOBm FbFi.
One liter of water dissolves 0.6 gm. PbFi at 9*, 0.64 gm. at 18°, and a68 gm. at
36.6' (conductivity method). ' (KoUmusch. ijsS.)
100 cc. anhydrous hydrazine dissolve 6 gms. PbFi at room temp, with decom-
podtioO. (WeUi ud BrodBim, rgis,)
Freenng-point data (solubility, see footnote, see p. i) for mixtures of PbFt and
Pbli are given by Sandonnini (1911); for mixtures of PbF] -j- PbO by Sandoo-
nini (1914); for mixtures of PbFi + Pbi(POJ, by Amadari (191a), and lor
PbFi + NaF by Puchin and Baskow (1913).
LKAD FORMATE
35«
LEAD FORMATE Pb(HCOO)>.
Solubility of Lead Formats in Aqueous Solutions of Barium Formats at 25^
(Fock, 1897.)
Mol. %m SolutioD.
Gnuns per Liter.
O
0.29
0.74
^•24
2.91
S-92
100
Ba(HC0|),.
100
99.71
99.26
98.76
97.09
94.08
O
Pb(HC0,)i.
• • •
1. 104
2.803
5-309
11.42
23.11
28.3s
Ba(HC0|)s.
28.54
28.65
28.90
32.24
29.29
28.13
Sp. Gr. of
Solutions.
In SoUd Phase Mol. % of
Pb(HCO|)|.
Z
I
I
I
I
I
I
2204
2213
2251
2529
2341
23SS
0911
o
1.72
S-29
11.94
24.81
56.54
100
Ba(HCO|)a.
100
98.28
94.71
88.06
75 19
43 46
o
LEAD HYDROXIDE Pb(OH},.
S(x.uBiLiTY OF Lead Hydroxide in Aqueous Solutions of Sodium Hydroxide.
(Moist Lead Hydroxide used, temperature not given.)
(Rubenbauer, xQoa.)
Amount of Ns
Amt. of Pb
Mol. DQution
Gnuns per loo cc. Solution.
in aocc.
in 20 cc.
of NaOH.
NaOH. Pb(OH)s.
0.2024
O.IOI2
2.27
1-759 0.590
0.3196
0.1736
1.44
2.778 I. 010
0.5866
0.3532
0.785
5.10 2.056
0.9476
0.4071
0.485
8 235 2.370
1.7802
0.5170
0.258
15-470 3-010
LEAD lODATE Pb(IOt)>.
One liter of water dissolves 0.0134 S^* Pb(IOi)t at 9.2^, 0.019 gm. at 18^ and
0.023 gm. at 25.8**. (KohlAusch, 1908; BOttger. 1903.)
One liter HiO dissolves 0.0307 gm. Pb(IO|)i at 25®. (Harkins and Winninghoff, igzz.)
Solubility of Lead Iodate in Aqueous Salt S(x.utions at 25®.
(H. and W., 19x1 )
Gms. ]
per Liter.
PbdO,.
Gms. per
liter.
Gms. per
Liter.
KNQ,.
KIO,.
PbCIO,),.*
'Pb(NO,),.
Pb(IQi),.
0.202
0.0318
O.OII3
0.0199
1.656
0.0052
I. Oil
0.0363
0.0227
0.0122
16.561
0.0045
5-055
0.0567
Pb(N0,),.
82.805
0.0078
20.220
0.0708
0.0165
0.165
0.0242
O.OII5
496.83
0.0418
SAD IODIDE Pbl,.
Solubility
IN Water.
(Lichty, 1903.)
f.
Density.
Grams Pbli
per 100.
Millimols PbIt per xoo.
(H,0 at ©•.)
cc. Solution.
Grams H<0.
cc. Solution.
Grams U|0.
0
1.0006
0.0442
O.C442
0.096
0.096
15
0.9998
0.0613
0.0613
0.133
0.133
25
0.9980
0.0762
0.0764
0.165
0.166
35
0.9951
0.1035
0.1042
0.224
0.226
45
0.9915
0.1440
0.1453
0.312
O.3IS
55
0.9872
0.1726
0.1755
0.374
0.381
65
O.Q827
0.2140
0'.2i83
0.464
0.473
80
0.9745
0.2937
0.3023
0.637
0.656
95
0 9671
0.3814
0.3960
0.828
0.859
100
• . •
0.420
0.436
0.895
0.927
Data for the solubility of lead iodide in water by the conductivity method are
given by B6ttger« 1903; Kohbrausch, 1904-05; Denham, 1917.
3S9 LKAD lODIDB
SCLUBILITT OF MiXTUSBS OP LBAD IODIDB AND POTASSIUM lODIDB IN WaTBR.
(Ditte, 1881; Sdutiiiauken, 1893.)
Gms. per 1000 Gins. HyO. « kj »i„ m * Gms. per 1000 Gms, ^O. _ .. . ^^
• .
' Pblf
KL
^ ouua rt
m^
tr .
Pbl,.
KI. "
wKi rmm
5
• • ■
163
Doobfe Sdt+PUt 50
526.7
1906 Doobk Sah+KI
.20
9
260
•
64
789.3
2161
tt
2S
25
325
M
83.5
i,xo8.6
2434
<•
39
45
449
M
92
1,273
2566
••
67
255
751
M
137
2,382
3278
M
80
731
1186
M
165
4,187
4227
M
80
569 9
976..
♦
2X8
10^03
• • •
«•
104. 5
1411
1521
M
241
12,803
7998
m
120
2151
1812
••
242
12,749
• • •
«•
137
2874
2097
M
250
15,264
• • •
m
17s
5603
2947
M
157
5,218 gms. Pb^sKI PbI«.aKLai^O
189
• • •
3339
••
172
6489 "
•(
M
9
96.6
1352
M
+KI
186
7,903 "
••
M
13
114. 3
1384
«•
M
194
9,266 "
«i
M
23
186.3
1510
••
•«
201
11,320 "
••.
M
. 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 0.002 16 gm. mols. Pbit (0.996
gms.) at 20^ (Fedotieff, 1911-11-)
SOLUBILITT OF LBAD IODIDB IN ACBTONB, AnILINB AND AmTL AlCOHOU
(von LaascvynakL 1894*)
G«]«»* 4a Gms. PbIt per xoo
(CH3)iC0 59 0.02
CatNHi 13 0.50
CsHsNHa 184 I. ID
QH7OH 133.5 002
SoLUBiLnT OF Lbad Iodidb in Ptbidinb.
(Heise, 19x3.)
Gms. Pb]^ Gms. Pbl|
t*. perxooGmt. Solid Phue. t". perxooGms. Solid Plan.
Pyridine.
—43 • 5 f -Pt- . . . PbVaCjao^
—37 0.166
—20 0.175 "
— 9 0.186
o 0.200 "
+ 3 0.215
6tr.pt. 0.225 Pb]^.3CfHiN+Pb]^.9C;BiN
15 0.208 Pb]^.aCaiiN
100 gms. 95% formic acid dissolve 0.25 gm. PbIt at I9.8^ (Ajchan, 19x5.)
100 cc. anhydrous hydrazine dissolve 2 gms. Pbli at room temp, with decom-
position. (Welsh and Brodenon, 191 5*)
Freezing-point data for miirtures of lead iodide and silver iodide are giveo
by Matthes (191 1).
LKAD MALATE Pb.C4H4Os.3HA
Solubility in Water and Alcohol.
(Parthdl and Habner, 1903.)
100 gms. HiO dissolve 0.0288 gm. PbC4H40i.3HiO at 18"*, and 0.06504 gm. at
35*.
100 gms. 95%.alcohol dissolve 0.0048 gm. PbC4H^i.3HtO at iS'^-as^
Density of alcohol employed » 0.8092.
35
Pyridine.
0.188
PbI|.aGAN
57
77
0.190
0.228
M
92
98
0.290
0.340
M
M
105
108
0.370
0.410
M
U
112
0.445
M
LKAD LAU&ATE
360
LEAD LAU&ATE, MTRISTATE, PALMITATE and STEARATE.
SOLUBILITT OF EaCH IN SEVERAL SOLVENTS.
G^acobson and Holmes, 1916.)
(See Lithium Laniate, p. 375, for fonnulas and other details. See also p. 363.)
Solvent.
t".
Gms. of Each Salt (Determined Separately) per 100 Gmi.
Solvent.
Water
u
Abs. Ethyl Al(X)hol
II
u
u
((
(t
a
Methyl Alcohol
u
u
u
«
Ether
Ethyl Acetate
it
ii
i(
Pb Laurate.
Pb Myri»tAt4<(.
PbPalmiUte.
Pb Stearate.
35
0.009
o.oos
0.005
0.005
50
0.007
0.006
0.007
0.006
25
0.009
0.004
0
0
35
0.032
0.004
O.OOI
O.OOI
50
0.264
0.052
0.012
0.004
155
0.061
• 0.056
0.051
0.039
25
0.096
0.078
0.069
0.051
35
O.II3
0.082
0.076
0.062
50
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
003s
0.015
0.009
0.008
50
0.201
0.077
0.033
0.020
15
O.OII
O.OIO
0.009
0.008
Benzene
LEAD NITRATE Pb(NO,)s.
Solubility in Water.
(Mulder; Kremers, 1854; at 15% Michel and Kraft, 1854; at Z7^ Euler, 1904.)
MM
Grams Pb(NO,)s per i
:oo Gms.
Grams Pb(NQi)t per zoo Gnw.
Ill _A
V,
Water.
"1
Solution.
27-33^^
4 . *"
Water.
Solution.
0
36.5^'>
38. 8 W
40 69.4
75
41.9
10
44.4
48-3
316
50 78.7
85
45
17
SO
54
34.2
60 88
95
47.8
20
52.3
565
35.2
80 107.6
"5
527
25
56.4
60.6
36.9
100 127
138.8
571 ,
30
60.7
66
38.8
17 52.76*
34 54*
• Euler.
(i) Mulder.
(2) Kremers, (3) Average at M and K.
Density of saturated solution at 17'' » 1.405. (Euler.)
100 gms. HsO dissolve 55.8 ems. Pb(NOs)s at 20®. (LeBlanc and Noyes, 1890.)
100 gms. HjO sat. with Pb(NOi)j + KNOt at 20* dissolve 95.39 gms. Pb(NOt)i.
+61.05 gms. KNOt. (LeBlanc and Noyes, 1890.)
100 gms. HiO sat. with Pb(NOi)i + NaNOi at 20** dissolve 38.42 gms. Pb(NOt)i
+84.59 gms. NaNOi. (Le Blanc and Noyes, 1890.)
Solubility of Lead Nitrate in Aqueous Solutions of Copper Nitrate
AT 20*.
Fedotieff, zgiz-za.)
. « c ^ o I Gms. per zoo Gms. HtO*
Gms. per zoo Gms. HsO-
Cu(NOj),.
Pb(NO,)»:
010 ***^ om. o<
0
55-11
1. 419
7.7
39-34
1-354
1504
27.80
1.322
24.63
19 05
1. 321
33-25
14.70
1-343
Cu(N(V)|.
37-96
60.32
83.11
100.29
127.70*
PbCNO,),,
13-08
8.19
5-37
3-53^
2.33*
* Solid phase in contact with this solution - Pb(NQ^x + Cu(N()^|.6H^.
dn of Sat. Sol.
1.360
1. 451
1.546
1.622
1.700
36i
LEAD NITEATE
Solubilitt'of Lbad 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 Sodium Nitrate as
Solid Phase.
Results for Lead Nitrate as
Solid Phase.
f of
Cms. per 100 Cms. Sat. Sol.
Saturation.
' NaNOb. PbCNQ,),.
32
34.42 19.69
35S
34.15 20.33
39. S
33-71 21.3s
44
33 35 22.19
49.x
32.94 23.15
55
32.60 23.93
58
32.47 24.24
62
32.33 24.57
65
32.19 24.89
f of
Gms. per loo Gma. Sat. SoL
Saturation.
NaNOk.
Pb(NQ,),:
21
40.97
13.62
26. s
42.04
13-38
31
43.18
12.88
38.8
44.63
12.78
4X
45."
12.94
44.25
46.03
X2.45
51
47.28
12.50
58
49.03
ZI.76
64
49.92
IX. 56
Solubility of Mixed Crystals of Lead Nitratb and_Strontium Nitrate
in Water at 25*.
(Fock. 1897.)
Mol. percex
It in Solution.
Gms. per 100 cc. Solution.
Sp. Gr. of
Solutions.
Mol. per oen(
. in Solid Phase
Pb(N0i)i.
Sr(NQi)s:
Pb(NQ,),.
Sr(N0,),.
Pb(NOj),.
SrCNQ,),.
100
0
46.31
0
1.4472
100
0
87.41
12.39
50.47
4.56
1.4336
99.05
0.95
78.68
21.32
53.92
8.14
1.4288
98.11
1.89
56.39
43.61
45.34
17.81
1.4263
97.02
2.98
60.29
39. 71
44.48
X8.74
X.4245
96.06
3-94
33.70
36.30
25.23
35.03
1.4468
83.84
16.16
24.58
75.42
19.13
37.54
1.4867
32.88
67.1a
0
100
0
71.04
I.5141
0
xoo
Solubility of Lead Nitrate in Ethyl and Methyl Alcohol.
Solvent.
Gms. Pb(NQi)i per 100 Gms. Solvent at:
/ " \
Aq. CsHftOH (Sp. Gr. 0.9282) 4 . 96 5.82 8.77 12.8
Abs. CsHftOH 0.04 (20. 5^) ...
Abs. CHiOH 1.37
so-
14.9 (G)
... (de B)
• • • • • ■
(Gerardin, 1865; de Bnqm, 1892.)
100 CC. anhydrous hydrazine dissolve 52 gms. lead nitrate at room temper-
ature with formation of a yellow precipitate. (Wekh and Brodenon, 19x5.)
Solubility of Lead Nitrate in Pyridine.
(Walton and Judd, 191 1.)
GnM. PbCNOOi
Gms. Pb(N0a)i
t". per xoo Gms.
Solid Phase.
t".
per xoo Gms
SoKd Phase.
Pyridine.
Pjrridme.
-19.4 2.93
Pb(NQi)s4CiH|N
45
22.03
Pb(N<X)s.4CiH|N
-14.S 2.14
((
49-97
29.37
(1
— 10 1.90
(f
51 tr.pt
• • •
" +Pb(NQi),.3CiH,N
0 3.54
M
59.5a
36.70
Pb(N0i),.3r4H,N
5.4 3-93
M
70
47-29
M
8.7 5.39
M
80
6Z.60
M
14.72 6.13
M
89.93
90.21
M
19.97 6.78
M
94 94
128.06
«
24.75 8.56
M
96 tr. pt.
• • •
** +3Pb(NQi),.aC4H,N
30.03 10.98
M
99 89
143.36
3Pb(N0b)s.3CAN
34.97 13. »
M
104.90
152
M
40.Q3 16 94
M
109.90
163.80
M
LKAD MITSATK 363
Solubility of Lead Nitratb-Nitrite, Pb(N0t)t.Pb(N0t)i.2Pb(0H)i.2Hi0,
IN Aqueous Solutions of Acetic Acid at I3.3^
(Chiksotti, 1908.)
Nonnaliftyof
Acetic Acid
Grns. PbO per 100
cc. Sat. Sol.
Normality of
Acetic Add.
Gms. PbO per 100 cc.
Sat.SoL
0
0.601
0.25
S-4SO
0.05
I 323
0.50
9.690
O.IO
2.18s
0.7s
1.5. 874
LKAD OXALATE PbC,0«.
One liter of water dissolves 0.00x5 §rni. PbC,04 at 18® (conductivity
method) . (BOttser — Z. phyak. Chem. 46^ 6oa, '03; Kobliaiiacli — Ihid. 5(H 356. 'o4-'o5.)
LIAD 0ZID18. Solubility in Water.
(BGtt0er; Ruer — Z. anorg. Chem. 50^ 373, '06.)
No. DeKiiplion of Oxide. ^^^J pc?Litir.
1. Yellow Oxide, by boiling Pb hydroxide with 10% NaOH i . 03 X lo""* o. 023
2. Red Oxide, by Doiliag 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® i.ooXio""* 0.022
5. Yellow Oxide, by heating com. yellow brown oxide to 620** i . 09 X 10"* o. 024
6. Yellow Brown Oxide commercially pure i.ioXio*"* 0.024
7. Yellow Brown Oxide, by long rubbiag of No. 5. 1.12X10""* 0.025
Bottger gives for three samples of lead oxide, 0.0x7, 0.021, and 0.013
gm. per liter respectively.
One liter H/) dissolves 0.068 em. PbO at I8^ solid phase PbO and 0.1005 gm.
PbO at l8^ solid phase PbsOs(OH)i. (PleiBBiier. 1907.)
Results for the solubility of hydrated lead oxide in water and dilute HtSOi
solutions are given by Sehnal (1909). The results are considerably higher than
the above, viz. 0.1385 gm. Pb per 1000 cc. HfO at 20''; with increase of H1SO4
the solubility decreases rapidly.
100 cc. anhydrous hydrazine dissolve i gm. lead oxide (red) at room temp.
(Weuh and Broderson, 191$.)
Freezing-point lowering data for mixtures of PbO + PbS04 are given by
Schenck and Rassbach, 1908. Data for mixtures of PbO + SiOs are given by
Weiller, 191 1, and by Cooper, Shaw and Loomis, 1909.
LKAD PerOXIDE PbOs.
The two forms of lead superoxide, (a) amorphous and (5) crystalline, differ
in their solubilities in sulpnuric acid. One liter of very concentrated HiSO
dissolves about o.oio mol. PbOi (b) at 22^. One liter of cone. HtSOi contain-
ing 1720 gms. per liter, dissolves 0.099^ mol. PbOi (a) at 22^ The solid phase
is slowly converted to PbCSOOs. One Titer of H1SO4 containing 1097 gms. H1SO4
per liter dissolves 0.004 "lol. PbOi at 22®. The solid phase is converted more
quickly to Pb(S04)s. In more dilute HtS04 solutions no solubility can be de-
tected. (Doksakk and FinckE, 1906.)
LKAD PALMITATE, LKAD STKARATK. See also p. 360.
100 cc. absolute ether dissolve 0.0138 gm. palmitate and 0.0148 gm. stearate. '
(lidoff, 1893^)
LIAD TetiaPHENYL Pb(C«H«)«.
Freezing-point daU for Pb(C«Hi)4 + Si(C«Hi)4 are given by Pascal (1912)-
LKAD PHOSPHATE (Ortho) Pb.(P04)s.
One liter water dissolves 0.000135 gm. lead phosphate at 20* by conductivity
method. (B6tt«erp 1903.)
One liter of 4.97 per cent aqueous acetic add solution dissolves 1.27 gms.
Pb,(P04)i. (Beftimnd, z8680
363 LEAD SUCCINATI
LEAD SUCCINATE PbC«H/)4.
Solubility in Water and in Alcohol.
(Paithea and Habnefp 1903.)
100 gvoB. H]0 dissolve 0.0253 gm. PbC4H404 at 18^, and 0.0285 8^- ^t 25^
100 gms. 95% alcohol dissolve 0.00275 gm. PbCiHiOi at 18'', and 0.003 gm.
at25^
Density of alcohol used » 0.8092.
Solubility of Lead SucaNATs in Water.
(Cantoni and DioCalevi, 1905.)
t*. xo*. ax*. 3a*. 39*. 50*.
Gms. PbC4H404 per loo cc.
sat. sol. 0.015 0.019 0.024 0.027 0.029
LEAD SULFATE PbSOi.
Solubility in Water.
(Average curve from gravimetric results of Dibbits (1874), Beck and Steg*
mflller (1910) and Pleissner (1907) and conductivity results of B6ttger (1903)
and Kohlrausch (1904-05).
f.
Gms. PbS04 per LUer.
0
0.028
s
0;03I
10
0035
IS
0.038
18
0.040
f.
Gms. PbS04 per Later.
20
0.041
25
0.04S
30
0.049
35
0.052
40
0.056
Results considerably higher than the above are reported bv Sehna! (1909).
This author finds 0.082 gm. PbSOi per liter at 18^ and claims that the presence
of HtS04 in the PbSOi reduces the solubility very greatly. His results for the
solubility in presence of small amounts of HfS04 are:
Gms. HtS04 per 1000 cc. solu-
tion o 0.0098 0.0196 0.0980 0.4900 0.9800
Gms. dissolved PbS04 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 HfSOi
solutions is exactly the same at 100* as at 20^.
Data for the solubility of PbS04 precipitates are given by deKoniack, 1907.
S(X.ubility of Lead Sulfate in Aqueous Solutions of Ammonium Acetate
AND op Sodium Acetate.
(Npyes and WUtoomb, 1905; Dumungton and Long, 1899; Dibbits, 1874.)
In Ammonium Acetate. In Sodium Acetate.
At 25* (N. and W.). At 100' (D. and L.). (D.).
Uminob per Liter. Obh. per Littr. G.NH«C»HA G.PbSO« Gaa. perioo Gna. H^.
KH4C.HA. PbS^T NH«CAb|. PbS04. "ShStSS!' SJSn'' NaCHA- PbSO*.
o 0.134 o 0.041 28 7.12 2.05 0.054
103.5 2-IO 7.98 0.636 32 9.88 8.2 0.853
207.1 4.55 15.96 1.38 37 10.58 41 11.23
414. 1 10.10 31*92 3.02 45 II. 10 I
Solubility of Lead Sulfate in Aqueous Solutions of Ammonium
Acetate at 25*.
(Maiden, 19x6.)
Qua, per 1000 Gms. S>tt. SoL Gms. per xooo Gma. Sat. Sol. j ^c.* CaI
HH4CAO,. PbSOT* NH4C»H|0t. PbSOjT i»«Sat.5oL
7.96 0.636 53.4 5.60 1. 012
15.91 I-370 106.8 16.8 1.024
31.70 3.04 213.7 38.9 1.045,
(I
M
(I
((
U
UAD SULFATE 364
Solubility of Lead Sulfate in Aqueous Solutions of Potassium Acbtatb
AND OF Sodium Acetate at 25^. (Fox. 1999.)
In Aq. Potassium Acetate. In Aq. Socfium Acetate.
Gms. per xoo Cms. Sat. SoL Cms. per xoo Cms. Sat. Sol. c^i. •
^ * N Solid Phase. , *■ v 5u
CHiCOOK. (CH,C00)«Pb. CH,C00Na. (CH,C00),Pb. NatSO^. *^****^
4-33 2.54 PbS04+PbK,(S04)i 6.69 0.78 0.34 PbSQ,
903 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 CHiCOOK solutions, the double salt PbKsCSOOi 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 StegmOller, zgio.)
In Aqueous HCl. '^"^-^^"^ "" M^'
>^ Milligrams Pb per xoo cc. Sdution. Normal- Mgm. Pb Normal- Mem. Pb
Normality , ^ it^ pcrioocc ityof pcrioocc
ofHa. y^^jg. ^j,j. ^4 3^0 ^Q^ Sol. NaQ. Sol.
o(=spureH20) 2.60 3 3.80 0,1 10.48 o.i 11. 19
o.i 19 22.18 28.04 0.2 17.48 0.2 18.73
0.2 35.70 42.88 54.50 0.3 23.41 0.3 36.51
0.3 55.37 65.15 84.04 0.4 29.84 0.4 33.76
0.4 75-27 88.80 III. 90
Solubility of Lead Sulfate in Aqueous Solutions of Sulfuric Acid
AT 18**. (Pleismcr, 1907.)
( See also Sehnal, preceding page.)
Gms. per Liter. Millimols per Liter. Gms. per Liter. Millimols per Liter.
HtS04. ' PbSOT H1SO4. PbSO*: ■ H,S04. ' PbSO*. HiSO*. PbSO*.'
o 0.0382 o 0.126 0.0245 0.0194 0.25 0.664
0.0049 0.0333 O-OS o.iio 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.
(SchulU, i86x; Rodwdl, z86a.)
In Aq. H,S04. In Aq. HCl. In .Aq. HNO|.
(a) (6) (c) (a) (6) (c) (a) {b) (c)
1.540 • 63.4 0.003 1.05 10.6 0.14 1.08 II. 6 0.33
1-793 85.7 o.oii 1.08 16.3 0.35 1. 12 17.5 0.59
1.841 97 0.039 I. II 22 0.95 1.25 34 0.78
I. 14 27.5 2. II 1.42 60 I. 01
I. 16 31.6 2.86
(a) Sp. Gr. of Aq. Add. (fi) Gms. Acid per zoo Gms. Solution, (c) Gms. PbSOi per 100 Gms. Solvent.
Solubility of Lead Sulfate in Conc. Solutions of Sulfuric Acid.
(Donk, 19x6.)
Gms. per xoo Gms. Gms. per xoo Gms/ .
f. Sat, Sol. Solid Phase. f. S>t- Sol. ^
H,S04. PbS0«. H,S04. PbSO*.
O 51.2 O PbSO* 100 61.2 O PbS04
O 89.4 O " +H,S04.Ht0 100 72.5 O.I
O 97 O H,S04 ICO 96.3 0.2 "
O 97.2 0.3 " +PbS04 ICO 99.1 0.9 "
50 .50.4 O PbS04 200 79 O "
50 '86.7 O.I " 200 88.8 O.I
50 95- 1 0.2 " 200 95.5 0.3
50 99.3 0.6 " 200 98.9 I.I "
Additional data for highly concentrated solutions of HtSOi are given by Ditz
and Kanhattser (1916).
365
LBAD SULFATE
Solubility op Basic Lead Sulfates in Water at iS"".
Cranpouiid.
} Basic Lead Sulfate
f Basic Lead Sulfate
(Plc
Fonnula.
1907.)
One Liter Sat. Solution Contains:
Mg. Lead Salt « Mg. Pb
PbS04.PbO 13.4 10.6
PbS04.3PbO.H,0 26.2 22
MillimobPb.
0.050
0.106
LBAD PerSULFATE Pb(SO«)s.
Solubility in Aqueous Sulfuric Acid at 22^.
(Doleialek and Finckli. 1906.)
Gma.
per Liter.
Solid Phase.
Gm
1. per Liter.
H.S04.
Pb(S04>t.
H,S04.
PbCSO*),.
948
0
Pb0S0«.Hi0
I2S3
14-85
IOI4
0.719
«<
1352
16.17
I081
1. 198
«
1470
930
1098
I.SS7
M
1532
9.46
1 130
2. IIS
«
163 1
19.80
I180
S-749
M
1698
33-34
I217
9 303
U
1703
35-22
Solid PhaM.
Pb0S04.H^
i<
Pb(S0|)i
11
M
M
The solid phase at concentrations of add up to 1352 gms. per liter is the white
basic ^t of the composition FbOSOi.HiO. In the concentration limits of
about 1470-1703 gms. HtS04 per liter the original yellow color of the solid phase
remains unchanged.
Freezing-pbint data (solubility, see footnote, p. i) for mixtures of PbS04-HLiiS04,
PbS04 + R>S04 and PbSOi + NatS04 are given b^ Calcagni and Mariotta (1912).
Results for mixtures of PbS04 + K1SO4 are also given by Grahmann, 19 13.
k.
£EAD (Hypo)8ULrATI.
Solubility op Mixtures op Lbad Hyposulphatb and Strontium
Htposulphatb at 25®.
CPock — Z. Kryit. Min. iB, 3^ '97-)
llbi. pef ceot hi Sohitioo.
PbS^Oa
•4HiO.
0.0
I. OS
IS 31
46.80
62.30
75 -75
78.09
88.29
100. o
Grams per liter.
PbSM.
SrSiOft.
Sp. Gr. of
Itttions.
sp.
£1
Mol. per cent in Solid Phue.
100. o 0.0 145*6 1.1126
98.9s 2.97 151.2 I.I184
84.69 40.82 152.5 I 1503
53.20 149-2 II4-5 I -2147
37.70 256.1 85.0 1.2889
24.25 310.3 67.0 1.3252
21.91 373.7 708 1.3726
11. 71 509.5 45.6 I. 4671
0.00 374-3 0.0 I. 6817
LEAD SULFIDE PbS.
One liter HtO dissolves 3.6. lo"^ gm. Mols. =» 0.00086 gm. PbS at 18'
Determined by conductivity method. See also Bruner and Zawadzki (1909).
Fusion diagrams for PbS -H ZnS and PbS -|- AgjS are given by Friedrich
(1908). Results for PbS + SbtSi are given by Wagemmann (1912).
LEAD SULFONATES. solubility in Water.
Name. Formuht. *•- S^gSI l£o. Authority.
.4HjO.
00
0.30
3 87
9-84
19.26
23 -73
32.24
49-97
0.00
SrSsOt
.4H«0.
100. 0
99-7
96.13
90.16
80.74
76.27
67.76
50-13
0.00
(Weigel, 1907.)
Lead 2.5 Diiodobenzenesulfonate CuIWl4S|Pb.4HiO 20
Lead fi Naphthalene Sulfonate (CioH7SOk)sPb.HfO 25
" a " " (CiBH7SQi),Pb.aH,0 24.9
Lead 2 PhenanthieneMonosuIfonate iHiO 20
S " " 3H,0 20
10 *• " 4H1O 20
M
if
0.77 (Boyle, 1909.)
0 . 4 (Witte, '15; Ettwn, '09.)
4.19s (Euwes, 1909.)
0.014 (Sandqnist, 1919.)
0.08
0.14
M
UAD TABTEATE
366
LEAD TAETEATE PbC^OJI^.
Solubility in Water.
(Caatooi And Zuboder — BiiU. loc. chim. [3] 33> 75i. '05*. Puthefl aad HQliMr — AtcUt. Phum. 241;
413, '03.)
18
35
40
>bO<VH4pcr
X. Soluaon.
Gms. PI
100 cc.
O.OIO (P. and HO 50
0.0108 " 55
0.00105 60
0.0015 65
Gms. PbCLOcHi per
100 cc. Solttdan.
Gms. PbCOA per
100 cc. aolttdon.
70
75
80
8S
0.0032
00033
0.0038
00054
0.00225
0-00295
o. 00305
o. 00315
Note. -— The positions of the decimal points here shown are just
as given in the original communications.
100 gms. alcohol of 0.8092 Sp. Gr. (about 95%) dissolve 0.0028 gm.
PbC40eH4at I8^ and 0.00315 gm. at 25**. (p. ^^ g.)
LECITHIN C4sHa4NPOt.
too ems. of sat. solution in aqueous 5% bile salts contain ^.5 gms. lecithin at
15^-20 and 7 gms. at 37^. Lecithin is practically insoluble in water.
(Moon, WilMB Md HiitfhiMon, 1909.)
LEUCINE CH,(CH,),CH(NH,)COOH.
too cc. HiO dissolve 2.2 gms. leucine at i8^
100 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 Wttrgler, 1914, and Pfeiffer and Wflrgler, 1916.
UGNOCERIC ACm.
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.
UGB&IN.
100 cc. HiO dissolve 0.341 cc. ligrdin at 22*, Vol. of solution ■■ 100.34, ^P- ^f*
0.9969.
100 cc. Iigr6m dissolve 0.335 cc- HsO at 22^, Vol. of solution •■ 100.60, Sp. Gr.
0.6640. (Herz, 1898.)
LL
One gm. atom Li dissolves in 3.93 gm. mols. NH| at — 8o*, at —50*. at —25®,
and at o
(Ruff and GomI, 1906.)
ACETATE CH|COOLi.2HsO.
Freezing-point data for mixtures of lithium acetate and acetic add are given
by Vasilev, 1909.
SulfoANTIMONATE Li,SbS«.ioH,0.
Solubility in Water and in Aqueous Alcohol.
In Water. (Donk, 1908.)
Gms. LLSbS«
f*. per xoo Gmt. Solid Pbaic
«•.
In Aqueous Alcohol at 10^ and 30^.
Gnu. per 100 Gmt.
Solid PlMW. Antbority.
SS.
Sol.
Sat. Sol.
CAOH.
Li«SbS«.
- 1.7
7.1
Ice
10
10.7
41.8
Li|SbS«.xcHiO (Dank. 1908.)
- 3-2
12.8
II
10
26.2
36.5
II
M
- 5.x
17.5
II
10
66.2
20.6
M
M
— 10.8
23.2
M
30
13.3
46.3
LitSbS«.8|H«0
-159
28. s
l(
30
51-9
30.7
II
— 26. a
35. 3
II
30
54 8
29.9
M
(Schxein^.
-42
40.4
Ice+Li|SbS4.xoH,0
30
58:4
30.8
U
xnakeiBMid
0
45.5
LitSbS«.ioH,0
30
58.6
32.3
" +U|SbS4
Jacobs,
+10
46.9
M
30
65.26
29.31
Li|SbS«
1910.)
30
50.1
M
30
74.3
24.1
II
SO
SI.3
M
30
79. S
ao.s
M
1
367 LITHIUM BKNZOATK
LITHIUM BINZOATE CACOOLL
Solubility in Aqueous Alcohol Solutions at 25®.
(ScideU, 19x0.)
Per cent j ^ Gms. CACOOIi Per cent j ^ Gas. CACOOLi
CAOH in cf? qXi per xoo Gmi. CtlLOH in cT? Sj per xoo Gms.
--gj^ bat. SOL Sat. SoL SdTvent. !>«. boU Sat. SoL
o I. 103 27.64 60 0.970 19.80
10 1.088 28.60 70 0.932 15.40
20 1.072 28.50 80 0.890 10.70
30 1.052 27.80 90 0.847 6.40
40 1.030 26.20 95 0.823 4.50
50 1.003 23.60 100 0.799 2.60
100 gms. HsO dissolve about 40 gms. CcHfCOOLi at the b. pt. (U.S. P.)
too gms. alcohol dissolve about 10 gns. C«HtCOOLi at the b. pt. "
LITHIUM BORATE Li^DB/),.
Solubility in Water.
t^ o 10 20 30 40 45
Gms. LiaOBsOs per 100 Gms. H^ 0.7 1.4 2.6 4.9 11. 12 20
(Le Chatelier. 1897.)
Equilibrium in tme System Lithium Oxide, Bork OrmE, Water at 30^
(Dukebki, 1907.)
LhO.
BA.
^ Solid Phase.
' Li.0.
BA.
SdidPhaae.
7.01
■ • •
LiOH.H^
1.32
3.36
Li/).2BA^TV)
7.51
2.98
(1
0.86
2.47
(1
7.71
' 3.38
** +Li,O.BA.z6HiO
0.53
2.47
M
7.68
3.56
Li,0.BA.i6H^
2.17
13- 12
M
5.40
2.78
u
2.61
16.39
If
3.47
2.42
u
508
30.81
Li,0.5BA.zoHiO
2.94
2.51
u
4.10
27.07
«i
1.58
3.27
it
3.22
15.40
M
2.17
6.90
M
1.55
1540
M
3.66
14.78
«
1.30
14.14
M
525
22
M
0.96
11.47
B(OH).
5.63
23.8
II
0.63
4-85
it
1. 81
6.20
Li,0.aBA4PH/>
0
3. 54
u
Freezing-point data (solubility, see footnote, p. i) for mixtures of LiBQi
+ NaBOt, and LiBOs + LisSiOi are given by van Klooster, 1910-11.
LITHIUM BBOMATE LiBrO..
100 gms. HiO dissolve 153.7 gms. LiBrOi at 18^, or 100 gms. saturated solu-
tion contain 60.4 gms. Sp. Or. of sol. » 1.833. (Myliua and Funk, 1897.)
LITHIUM BBOUDB LiBr.2H,0.
Solubility in Water.
(Kremers, 1858; Bogorodaky, 1894; Jones, X907')
*•• SSciL^'lfio. SoUdPh.se. f. prdifl^O. SolidPb.se.
— 0.46 1.058 loeCJ) 10 166 LiBr.2H«0(K)
— 1.94 4- 274 " 20 177
— 4.27 8.678 « 30 191
— 10.3 17.80 " 40 205
""30.5 3764 " 44 209 « +LiBr.HiO (B)
—45 50 " +LiBr.3H«0 SO 214 LiBr. H,0 (K)
—30 80 LiBr.3HaO 60 224 "
— 10 122 " 80 245 "
O 143 " (K) XOO 266 "
+ 4 160 *< +LiBr.2H«0 (6) 159 ... IiBr.H^+LiBr (B)
Freezing-point data for LiBr + LiOH (Scarpa, 19 15), for LiBr -H AgBr.
(Sandonnini and Scarpii, I9X3')
100 gms. glycol dissolve 60 gms. LiBr at 14.7^ (de Coniack, 1905 J
II
M
tl
UTHIXJM CAMPHORikTE
368
DiLITHIUM d GAMPHORikTE CuHuOfLii.
Solubility in Aqueous Solutions of Camphoric Acid at 13.5^-16^
AND Vice Versa.
Gms. per xoo Cms. Sat. Sol.
CaKH Phsfl^
C|Hu(C00H)s. CuH,«0«lC.
0.621 0
Camphoric Acid
aHii(COOH),
2.02 3.77
(( ((
«
3.25 10.63
Monolithium Tetracamphorate
CioHu04Li.3CioUiA
3.51 12.61
(( ((
((
3.99 20.56
" Dicamphorate
CioHu04.Li.CioHi^4
3.43 24.69
«
2.87 37.16
" Camphorate
0 40.80
Dilithium Camphorate
CioHitOiLia
The mixtures were kept in a cellar at nearly constant temperature and shaken
from time to time until equilibrium was reached. Additional results at 17^-33^
are also given.
LTTHIUM CARBONATE LiiCO,.
Solubility in Water.
(Bevade, 1885; FlUddger, 1887; Draper, 1887.)
An average curve was constructed from the available results and the following
table read from it*
Gma. LitCOaper 100 Gms.
»o«
Water.
SdudoD.
0
1. 54
1.52
10
1-43
1.41
20
1-33
I-3I
25
1.29
1.28
30
1-25
1.24
Gms. liiCQ^pcr too Gma.
• .
Water.
Solutioii.
40
1. 17
1. 16
50
1.08
1.07
60
1. 01
1. 00
80
0.85
084
100
0.72
071
Density of saturated solution at o^ « 1.017; at 15*^ — 1.014.
Solubility op Lithium Carbonate in Aqueous Solxjtioks op
Alkali Salts at 25*^.
(Ge£Fcken — Z. anorg. Chcm. 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 liaCOs per lit^ in Aqueous Solutions of:
v^^^' mo..
O 12
10 12
20 13
30 13
40 13
60
80
100
120
140
170
300
TOO ems. aq
One Titer sat
63
95
10
25
40
KNO|.
2.63
3 05
3-3
3.6
3.S
3.8
3.6
35
3-3
3-0
2.6
2.2
KQ.
12.63
13.10
13 -5
13 -8
14.0
14.2
14.0
139
13-7
13 -3
NaQ.
12.63
13 -4
13 -9
143
14.6
14-5
14.4
14.2
14.0
KSSO4.
12.63
13 -9
14.7
154
16.0
16.9
17.7
18.2
NaiSO«.
12.63
14.0
15.0
16.0
16.6
17.8
18.6
19.4
19.9
20.4
NH«a. (NH«)sSO«.
12.63 12.63
16.0 20.7
19.2 25.0
21.5 28.2
23.3 30.8
26.0 35.2
27.6 38.5
28.4 41.0
28.7 42.6
28.8 43 S
28.9 •••
29.0 •••
056 gm. LiiCOi at 15.5*-
alcohol of 0.941 Sp. Gr. dissolve o. _ _
sol. in water contains 0.1722 gm. mols. » 12.73 ^s. LitCOi at 25*.
Ageno aad Valla, 19"^
369
UTHIXJM CARBONATE
Solubility op LirmuM Carbonate in Aqueous Solutions of Organic Com-
pounds AT 25®.
(Rothnwmd, 1908, xgio; Me also Tnube, 1909.)
The solubility in HiO " 0.1687 mols. LitCOt per liter » 1247 gms. at 25^*
Gm. Mob. LiiCOi per Liter in At). Sohitioo of:
■«■
Aqneoos Sdatkn of :
O.I3S
Noiaaity.
0.35
0.5
-^
*
NorauJUy.
Normality.
Normality.
Methyl Alcohol
■ • •
0.1604
0.1529
0.1394
Ethyl Alcohol
O.1614
O.I5SS
O.1417
0.1203
Propyl Alcohol
0.1604
0.1524
0.1380
0.1097
Amyl Alcohol (tertiary)
0.1564
0.1442
0.1224
0.0899
Acetone
0.1600
O.I5IS
0.1366
O.IIO4
Ether
0.1580
0.1476
0.1300
• • •
Formaldehyde
0.1668
0.1653
0.1606
0.1531
Glycol
0.1660
0.1629
0.1565
0.1473
Glycerol
0.1670
0.1647
O.1613
01532
Mannite
0.1705
0.1737
0.1778
• • •
Grape Sugar
0.1702
0.1728
0.1752
0.1778
Cane Sugar
0.1693
0.1689
O.1661
0.1557
Urea
0.1686
0.1673
0.1643
0.1605
Thiourea
0.1667
0.1643
0.1600
0.1523
Dimethylpyrone
0.1562
0.1460
0.1280
0.0992
Ammonia
0.1653
0.1630
0.1577
0.1466
Diethylamine
0.1589
O.I481
0.1283
0.0937
Pyridme
0.1592
0.1503
0.1347
O.IO9I
Urethan .
0.1604
0.1525
0.1377
O.III3
Acetamide
...
O.1614
0.1520
0.1358
Acetonitrile
O.1618
01556
0.1429
O.II78
Mercuricyanide
0.1697
0.1704
...
• . •
Freezing-point data for mixtures of LiaCOt + LitS04
(Amadori, 191 a.)
LiiCO, 4- K,CO,.
(Le Chatelier, 1894-)
(Bi) CARBONATE fclHCOk.
100 gms. H|0 dissolve 5.501 gms. LiHCOi at I3^
(Bevade, 1884.)
CHLORATE LiClO..
100 gms. HsO dissolve 213.5 gms. LiClOt at 18^, or 100 gms. sat. solution con-
tain 75.8 gms. Sp. Or. of sol. » 1.8 15. (Mylius and Funk, 1897)
100 gms. HiO dissolve 483'gms. LiClOi at 1 5°, du of sat. sol. » i .82. (Carlson, 19x0.)
UTHIXJM CHLORAURATE LiAuCU.
Solubility in Water.
(Rosenbladt, 1886.)
t*
Gms. LiAnCli per
r.
Gma. LtAuCl4 per
«•.
Gms. liAuCU pa
• .
100 Gma. SoltttKML
too Gms. SohitiOB.
zoo Gms. SohitXM.
10
53.1
40
67.3
60
76.4
20
57-7
SO
72
70
81
30
62.5
80
85.7
LrmUM GHLOBIDE 370
UTHIUM CHLOBIDB UCL
SOLUBILITT IN WatbH. (ATengB conv iiooi icnlte of Gerlach, 1869.)
f
Gms. LiQ i>er
100 GlBft.
V *
Water.
Soltttkm.
0
67
40.1
xo
72
41.9
20
78.5
44
25
81. s
44.9
30
845
45-8
t».
Gnii.ua
per 100 Gms.
Watw.
Soiutka:
40
90.5
47.5
SO
97
49. a
60
103
SI -9
80
"5
53-5
100
1275
56
Density of saturated solution at o^ 1.255; ^^ 15^ 1.275.
Solubility of LrrmuM Chloridb in Aqubous Solutions of Hydrochloric
Acid.
Results at o**. (Ei«d. 1888.) Results at 25*. CBeis, xgn-ia.)
Gms. per zoo cc. Sat. Sd.
LiCL
HCL
^ofSat. SoL
SI
0
I -255
41.4
8.2
1.243
28.5
24.1
1.249
24.6
29s
1. 251
ua.
HCL'
57-4
56.87
53.64
51.98
0
2.30
3.84
6.43
Solubility of LrrrauM Chloridb in Aqubous Solutions of Alcohol at 25*.
(Pinar de Rubies. Z913-1914.)
The LiCi was determined bv titration with AgNOi. Solutions saturated by
constant agitation for many nours. Solid pha^, LiCl.HiO for all mixtures.
The anhydride, LiCl, separates only from the most highly concentrated alcohol
solutions.
Gms. per 100 Gms. Sat Sd. Gms. per 100 Gms. Sat. Sol.
C|H«0H. ' LiCL CAOH. ' Ud.
o 44-9 50 25.75
10 40.9 60 21.6
20 37-25 70 21. 1
30 33-3 7S 20.8
40 29.4 80 20.75
Solubility of Lithium Chloridb in Ethyl Alcohch. at Diffbrent
Tbm PBRATURBS. (Tuzner and Bissett, 1913.)
«•• ''SL"^^^ Solid Pha*. r. • ^^*a^r Solid Phase.
o 14.42 LiCL4CsH50H 20 24.28 LiCl
S 15 04 " 30 25.10 "
10 16.77 " 40 25.38 "
IS 18.79 " 50 24.40 "
17 20.31 " 60 23.46 "
Solubility of Lithium Chloride in Sbvbral Solvents.
Gms.Lia Gms.Lia
So'^««t. Pg^ Amthority. Solvent. f. T^^ Authority.
Solvent. Solvent.
Alcohol: • Alcdiol:
Methyl 25 42.36 (Tomer 4 Biisett, 19x5.) Amyl 25 9.03 (Tomer ft Bimett, 19x3.)
Ethyl 35 2 . 54* (Patten ft Mott, X904.) " ? 7.2 (AndxewB&£nde.z895.)
Propyl 25 16.22 (Turner ft Binett, 19x3.) ** 25 9* (Patten ft Mott, X907.)
" ? 15.86 (SdJamp. X894.) Butyl 25 10.57*
" 25 3.86* (Patten ft Mott, 1904.) Glycerol 25 4.32*
Allyl 25 4.38* « " . Phenol 53 1.93* •*.
* Fosad LiCl used ior these determinaticns.
100 cc. anhydrous hydrazine dissolve 16 gms. LiCl at room temp.
(Welsh and Broderson, 19x5.)
M M
371
UTHnJM CHLOBIDS
S(X.UBOLiTT OF Lithium Chloride in Sbvbral Solvents.
(Laasc^ynaki, x894i' deConinck, 190$.)
In Acetone. (L.)
In Pyridine. (L.)
In Glycol. (deC.)
r.
0
Gma-Lia
per zoo Gnu.
(CHi)sCO.
4.60
46
Gms-Lia
per zooGms.
(CH,),CO.
3.76
15
Gdm. LiCI
per zoo Gms.
QHiN.
7.78
GniB.Lia
f*. per zoo Gms.
Sa.SoL
15 II
13
4.41
53
31a
100
14.26
25
4.II
S8
a. 14
S(X<UBiLiTY OP Lithium Chloride in Pyridine.
(Kahlcnhcig and Kiauakopf, 1908.)
In Anhydrous Pyridine. ^° 97% Pyridine + 3% Hrf)
Gma. Lia per zoo Gma. ^^ ^^^^
LiCLaCJEftN
«
LiCLCOtN
«
a
ii
Solubility of Lithium Chloride at 25* in Mixtures of:
f.
' Sftt. SoL Solvent.
8
H.31 12.71
28
11.87 13.47
40
11.60 13.10
60
11.38 12.84
80
11. 71 13.27
00
13.01 14.98
tr. temp, about a8*.
by Volume.
t*
Gms. LiCl
per zoo Gms.
Sat SoL
Solvent. '
22
12.50
14.31
33
13 -79
15.98
45
X5.58
18.46
S8
16.72
20.08
72
17.12
20.66
97
18.35
22.48
Acetone and Benzene.
(Maiden and Dover, 19Z7*)
Gms. Acetcme Gms. LiCl
per ZOO Gms. per zoo Gms.
Solvent. Solvent.
100
2.30
90
1.69
80
0.966
60
0.234
Gms. Acetone Gms. LiCl
per 100 Gms. per zoo Gms.
Solvent. Solvent.
40 0.088
20 0.019
10 0.009
O O
Ethyl Acetate and Benxene.
(Maiden and Dover, Z9Z7.)
Gms. Ethyl Acetate Gms. liQ
perzoo Gms. per zoo Gms.
Solvent.
Solvent.
100
1.78
90
80
0.147
0.028
70
0.005
Distribution of Lithium Chloride Between Water and Amyl
Alcohol at 30®.
(Dbar and DatU, zgzj.)
Mob. LiO per Liter.
fs.
ft
Mols. Lia per Liter.
a.
H|0 Layer cx.
Akohol Layer c«.
H^ Layer ci.
Alcohol Layer c«.
4
3.24
0.0347
93.37
2.68
0.0240
III. 66
3.06
0.0325
94.15
2.58
0.0275
113.40
2.93
0.0300
97.70
2.34
0.0200
117
2.82
0.0275
102 . 58
1.84
0.0125
147.2
2.76
0.0250
XIO.40
0.65
0.0030
216.66
Freezing-point data (solubility, see footnote, p. i) are given for the following
mixtures of Uthium chloride and other compounds.
Lithium Chloride + Lithium Hydroxide (Scarpa, Z9Z5.)
+ Magnesium Chloride (Sandonnini, z9z3. Z9Z4.)
4- Manganese Chloride (Sandonmni and Scarpa, zgza.)
-H Potassium Chloride (Richards and Mddrum, zgz;.)
+ " " -HJ^aCl (Richards and Meldrum,z9Z7.)
+ Rubidium Chloride (Richards IE Meldruia,'!?; Zemcxnsny ft Rainbach,'xa)
+ Silver Chloride (Sandonnini, Z9zza, Z9Z4.)
•\- Sodium Chloride (Zemcznsny and Rambach, 19Z0.)
-|- Strontium Chloride (Sandonnini, zgzz, z9zza, Z9Z4.)
+ Thallium Chloride (Sandonnini, z9zz, Z9Z4.)
+ Tin Chloride (ous) (Rack, 19Z4.)
CHBOHATE
372
LITHIUM CHBOHATl LisCr04.2H^.
UTHIUM BIOHBOMATS Li,CriO,.2HA
Solubility in Water at 30®.
(Sdutfnemaker— Z. phyak. Chem. 5s 79i '06; at i8*,Myliat uid Fvak-^Bcr.M i7i8iV7<)
GNDpontioii in
Weight per cent:
Solid
Pbaae.
OfSoltttiaii.
Of Residue.
%CrO».
%LijO.
%CrO».
%Li«0.
0.0
7.09
• . •
• • •
U0H.Htf0
6.986
7-744
4.322
18.538
M
16.564
8.888
10.089
19-556
M
25.811
10. 611
15 -479
21.106
m
33 618
12.886
24-365
19-393
M
37-411
14-306
44. 555
17. 411
IiOH.H«0 + LiiaO|.sH^
37 588
14-381
36 331
18-552
M a
37-495
13 3"
51-075
16.384
IkCiOt^E^
40.280
10.858
• « .
« • •
u
43.404
11.809
53-793
14 -070
LifCrOft^HsO + LisCkiO|.dbO
45 130
9-515
56.085
10-190
LisGrs07.sH^
47-945
7-951
58.029
9.238
••
57 -031
6.432
65.560
8-733
M
67-731
5-713
71.687
«-5i3
U^Ci^aB^ + Ci(H
67.814
5-689
80.452
3.780
M m
65.200
4.661
...
• • •
CrO*
63-257
2. 141
85.914
0.758
M
62.28
• ■ •
■ • •
• ■ •
«
A saturated aqueous solution contains:
49-985 per cent Li,Cr04, or 100 grams H,0 dissolve 99.9< grams
Li,Cr04 at 30** (S.).
56.6 per cent LijCr.O,, or 100 grams H,0 dissolve 1^0.4 crams
Li,Cr,0, at 30° (S.). '^ ^
52.6 per cent Li,Cr04, or 100 grams H.O dissohre iio.o grams
LiCrO^ at 18° (M. and F.). ^
Sp. Gr. of sat. solution at i8** — 1.574.
CITRATE C,H4(OH)(COOLi),.4Hrf).
100 gms. HiO dissolve 61.2 gms. Li citrate at 15^. dn sat. sol. « 1.187.
(Greenish and South, 1902.)
Solubility in Aqueous Alcohck. at 25*,
' (Seidell, 1910.)
insolvent.
Sat. Sol.
Gms.
CiTLpHCCOOU),.-
4H1O per xoo Gms.
Solvent.
Wt. %
diLOH
in solvent.
tf.of
Sat. Sol.
Gms.
CApHCCOOLOiv-
4H1O per xoo Gms.
Solvent.
0
1. 216
74.50
50
0.933
4.93
10
1. 150
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
965
100
0.788
0.02
373 UTHIXJM FLUORIDS
UTHIUM FLUORIDS LiF.
100 gms. HfO dissolve 0.27 gm. LiF at i8^ 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.
UTHIXJM FORMATE HCOOLL
Solubility in Water.
(Groaclraff, 1903.)
Gms. Mob. Qma. Mob.
Am HCOOLi HCOOU c^im pu.^ *• HCOOLi HCGOU SnWH P1»m*
^' periooGnia,i)«riooMol*. Solid Phoe. f. per too Gms. per 100 Mob. J^uO**™*-
Solution. HflO. H^. Bfi.
-30 31.14 9.28 HCOOUJa^ 91 54.16 40.90 HCOOLi JI^
o 24.42 ZI.18 " 98 57.05 45-99 HCOOLi
18 27.85 13.36 " 104 57.64 47.11 "
495 35-^ 1914 " 120 59.63 51.13 "
74 44.91 28.22 "
Sp. gr. sat. sol. at .iS*' » 1.142.
Solubility of Neutral Lithium Formate in Anhydrous Formic Acnx
(Groochuff, 1903.)
Gms. HCOOU Mob. HCOOLi
f*. per zoo Gms. periooMob. SoKd Phase.
Solution. lHCOOH.
o 25.4 30 HCOOLi
18 25.9 30.9
39 26.4 31.75
60 26.9 32.6
79 27.8 34
UTHIXJM HIPPXJR4TE CeHtCO.NHCH,COOLL
100 gms. HiO dissolve about 40 gms. of the salt at 15-20^
(Squire and Caioci, 1905.)
LITHIUM HTDROZmS LiOH.HA
Solubility in Water.
(Dittmar, z888; Pickering, 1893.)
it
ii
ii
Gms. par xoo Gms.
t* Solution.
Gms. LiOH
per zoo Gms.
H«0.
f.
Gms. per 100
Solution
Gms. Gms. LiOI
'• Der zoo Gm
LiiO
-
LiOH.
UOH. *W3.
— 10. 5
7.23
. . •
30
7.05
11.27 12.9
— 18 Eutec . . .
II. 2
...
40
7.29
11.68 13
0 6.67
10.64
12.7
SO
756
12.12 13.3
10 6.74
10.80
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
SULFOANTIlfONATE AT 30** AND ViCE VeRSA.
(Donk, 1908.)
Gms.i)eriooGins.
Sat Sol. Solid Phase.^
Gms.per
100 Gms.
Sol.
Sdid Phase.
LiOH. Li^SbSl. liOH. Li,SbS«:
II.4 0 LiOH.H/) 2.1 48.3
9.1 8.3 " 2.1 52,1
2.3 29.9 - 1.4 518
0 51.3
Data for equilibrium in the system lithium hydroxide, phenol,
given by van Meurs, 1916.
UOH.HdO
" +Li,SbS4.ioH/)
Li,SbS«.ioHdO
, water at 25*^ are
lODATE
374
lODATE Li(IOk).}H,0.
loo gms. HsO dissolve 80.3 gms. LilQs at 18'', or 100 gms. solution contain
44.6 grams. Sp. gr. of sol. a 1.568. (Mylius and Funk, 1897*)
UTHIXJM IODIDE
LiI.3H*0.
Solubility in Water;
(Kremen, 1858, x86o; ice curve, Jones, 1907.)
Gms. per zoo Gms.
•0.296
-I. 218
-2.70
6.14
-16.2
■25
-59
■69 Eutec.
■60
■40
-20
o.
10
Water.
1.08
4.36
8.71
17.69
38-31
48.67
85.13
93
100
118
134
151
157
Sat. Sol.
1.06
4.19
8.02
1503
27.70
32.72
46
48.2
50
54 13
57.27
60.2
61. 1
Solid Phase.
Ice
tt
tt
tt
tt
tt
tt
lce+LiI.3H,0
La.3H,0
tt
tt
tt
tt
so
25
30
40
SO
60
70
75
75
85
80
100
120
Gms. per xoo Gms.
Water.
I6S
167
171
179
187
202
230
263
m. pt.
m. pt.
435
481
590
Sat. Sol.
62.2
62.6
63.1
64.2
6|.2
66.9
69.7
72.5
81.3
82.8
85.5
So&d Phase.
La.3H,0
tt
tt
t*
tt
tt
tt
tt
tt
La.2HsO
LiLHsO
tt
tt
Solubility of Lithium Iodide in Several Solvents.
Solvent.
f.
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Amy! Alcohol
Glycol
Furfurol
25
25
25
25
iS-3
25
Nitromethane
0
u
25
* SoUd phase -
. LiI.4CJl70H.
CTumer and Biaaett, zgijO
II
M
M
343-4
250.8
47 52*
112. 5
38.9
45 -Qt
1. 227
2.52
t * gms. per zoo cc. sat. solution.
F.-pt. data for Lil + Agl are given by Sandonnini and Scarpa, 1913.
u
l<
M
(de Cooinck, 1905.)
(Walden, 1906.)
M
tt
UTHIXJM lODOMERCURATE 2LiI.Hgl2.6H,0.
100 gms. sat. solution of lithium iodomercurate in water prepared by cooline 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. H|0; Sp. Gr. of the sat. sol. « 3.28.
(Duboin, 1905.)
LITmUM LAURATE, MYRISTATE, etc.
Solubility in Water and in Alcohol of rf = 0.797, at 18® and at 25**.
(Partheil and Ferie, 1903.)
Formula.
C„H»COOLi
Ci«H„COOLi
CuHjTCOOLi
CHMCOOLi
CirHaCOOLi
(
Qms. Salt per xoo cc
M.
. Sat. Solution
in:
Salt
Water at
— \
Alcohol at
Stearate
Palmitate
Myristate
Laurate
Oleate
i8*.
0,010
O.OII
0.0232
0.158
0.0674
O.OII
0.018
0.0234
0.1726
0.1320
0.041
0.0796
0.184
0.418
0.9084
as*.
0.0532
0.0956
0.2100
0.4424
1. 010
375
LAURATB
LITHIUM LAUR4TE, MYBI8TATE, PALBOTATE and 8TEA&AT1.
Solubility of Each of thbsb Salts, Dbterminbd Separately, in
Several Solvents.
(Jacobooa and Holmes, 19x6.)
Li laurate = CnHnCOOLi. Li myristate — CiiHtTCOOLi, Li palmitate »
CH,(CH,),4C00Li and Li stearatc = CH,(CH,),«COOLi.
Excess of salt shaken with solvent for 2 hrs. in all cases. The sat. sol. was
Sdvoit.
Abs. Ethyl Alcohol
a
((
tc
u
ii
u
Methyl Alcohol
a
(t
Water
((
u
Ether
it
u
u
Amyl Alcohol
a
St
u
u
tc
tt
Chloroform
Amyl Acetate
tt
tt
tt
tt
tt
tt
Methyl Acetate
Acetone
tt
tt
drynesE
«•.
20
254
35
50
65
} and weighing residue.
Gms.of Each Salt (detennined ttpantdy) per
zoo Cms. Solvent.
Li
Lauimte.
0.403
0.447
0.546
0.782
1. 149
Li
Myristate.
0.194
0.224
0.278
0.43s
0.669
Li
PalmiUte.
0.096
O.I18
0.142
0.248
0.391
Li
Steaiate.
0.072
.0.089
0.106
0.200
0.333
15-2
25
34-6
SO
3159
3-773
4.597
6.038
1.346
i.68o-
2.193
3.281
o.6i6
0.771
1.086
1.652
0.349
0.439
0.658
1.057
16.3
25
35
SO
0.154
0.187
0.207
0.280
0.027
0.036
0.042
0.062
O.OIO
o.ois
0.015
• • •
0.009
O.OIO
O.OIO
• • •
158
25
O.OII
0.006
0.013
0.004
0.007
0.007
O.OII
O.OII
16
257
35
49.2
0.073
O.III
0.126
0.203
0.029
0.046
0.062
0.109
0.019
0.032
0.033
0.069
O.OII
0.028
0.031
0.060
152
0.006
0.004
0.004
0.004
14-5
25
35
SO
0.068
0.064
0.061
0.061
0.037
0.034
0.044
0.045
0.038
0.024
0.037
0.036
0.034
0.029
0.031
0.044
245
0.026
0.013
0.015
0.012
IS
25
35
0.300
0.376
0.430
0.413
0.447
' 0 . 502
0.434
0.508
0.537
0.571
0.706
0.663
^ 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.
TetraMOLYBDATE LitO.MoO1.2HtO.
100 cc. sat. aqueous solution contain 43.13 gms. LitO.MoOt.2HtO at 20^ dm
of sat. sol. « 144. (Wempe, 191a.)
NITRATE 376
NTnUTE LiN0t.3H<0.
«•.
Gnii.UNOb
per 100 Gna.
Solutioik
O.I
34.8
10.5
37.9
12. 1
38.2
13.75
39.3
19.05
40.4
22.1
42.9
27.55
47.3
29.47
53 67
29.78
55.09
cjBiLiTY IN Wat
)
Gnui. LiNOb
Solid Phase.
f.
per 100 Gins.
Sdtttion.
Solid Phase.
LiNa.3H/)
29.87
56.42
LiNQi.3Hrf)
29.86
56.68
(C
29.64
57.48
it
29.55
58.03
u
43.6
60.8
LiNQ..}HiO
50.5
61.3
it
55
63
tt
60
63.6
((
64.2
64.9
LiNO,
70.9 .
66.1
((
The eutectic Ice + LiN0i.3Hip, b at —17.8* and about 33 gms. LiNQj per
100 gms. sat. 80I. Transition points, 29.6^ and 61. i^
Data for the system LiNQi+LiiS04+HjO 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 20". (Roshdestwensky and Lewis, 1911.)
Freezing-point data for LiNOi + KNOi and LiNO» 4- NaNOi are given by
Carveth, 1898. Results for LiNOi + KNQs are also given by Harldns and Clark,
1915.
Results for LiNOi + LitSOi are given by Amadori, 1913,
UTHIXTM NITRXTl LiNO,.H,0.
SOLUE
IILITY IN WaTE
;r. (Oswald. 19x4.)
Gms.
Gms.
f.
LiNOi per
100 Gms.
Sat. Sol.
Solid Phase.
i.
UNOiprr
100 Gms.
Sat. Sol.
Solid Phase.
- 7.5
II. I
Ice
38.5
55.5
LiNOi.HdO
-II. 7
15
II
42
56.9
II
— 21
21.2
11
49
60.6
11
-28.8
29
II
49.5
61.2
« +LiNOfc.|HiO
-31.3
29.4
" +LiNOk.H/)
65
63.8
UNOk-iHiO
-19.3
33.9
LiNOi.HdO
81.5
68.7
11
0
4X.5
«i
91
72.4
II
+ 19
48.9W11-x.3iM.)
II
96
91.8
M
25
50.9
II
92.5
94.3
U
100 gms. H|0 dissolve 10.5 gms. AgNOi + 78.5 gms. LiNOi at 14^ (Oswald. 1914.)
UTHIUM OXALATE Li,CA.
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 xoo Gms. Solution. Mols. per xoo Mols. H«0. .... _.
Solid Phase.
H,CA.2Hrf)
HjCA-HjO and HLiC^4.H|0
Double Salt
HLiCrf)4.4H/)
»39.2HsCt04 and 44.7LiiC/)ii
HLiCA.HtO and LicC^4
5.87 ... 1. 901 LitCt04
100 gms. aqueous solution, simultaneously saturated with lithium oxalate and
ammonium oxalate at 25^, contain 5.75 gms. LiaCs04 + 4.8 gms. (NH4)sCi04.
XFooU and AndKW, 1903.)
' H,CO«.
10.20
10.66
10.55
Li,C04.
• • •
2.96?
3."$
H,C04.
2.274
2.457
Li,CA.
. . •
0.622
8.08
2.60
3.18
5.03
1.823
0.563
0.633 <
0.962 (
2.16
2.12
6. 54 J
1.61S
0.469
1.273
577 UTHIUM FR08PB4n
Lnnnni phosfeulti lupQi.
100 gms. HiO dissolve 0.04 gm. Li|P04. (M«y«r, 1856^
UTHIUM (Hypo) FHOSPB4n LuPsCXyHA
100 gms. HiO dissolve 0.83 gm. hypophosphate at ord. temp, (Runmdsbag. i89««)
UTHIUM PKEtMANQANATB LiMnO«.3HtO
100 gms. water dissolve 71.4 gms. permanganate at i6^ (Aahoff^
LITHIUM SALICYL4TI aH40HC00Li.iH,0.
Solubility in Aqueous Alcohol Solutions at 2^\
(Seiddl, 1909, 1910.)
Gms.
CAOHper
100 Gnn.
Solvent.
Gms.
tf.of QH^HCOOH.iHiO
Sat. Sol. per 100 Gms.
Sat. Sol.
Gms.
QHaOHper
100 Gms.
Solvent.
4iio(
Sat. Sol.
Gms.
CH40HCX)OH.»IW)
per too Gms.
Sat. Sol.
0
I . 209 56
60
1. 104
Sii
10
I 195 SS-9
70
1.083
49'S
20
I. 180 55.4
80
1.056
47. s •
30'
I. 163 54.7
90
1.026
45. 8
40
1144 SSI
92.3
1.020
45-6
SO
1. 124 52.5
100
1.027
48.2
100 gms. propyl alcohol dissolve 18.7 gms. Li salicylate (temp.?). (Schknp, 189SO
UTHIUM SULFATE LitSOi.HsO.
Solubility in Water.
(Aversge curve from Kiemers, 1855; Etard, 1894.)
M Gms. LiiSOi per m - ' Gms. Li|S04 per «• Gms. Li|SOi per
100 Gms. Solution. * * xoo Gms. Solution. * too Gms. Solution.
—20 18.4 20 25.5 SO 24.5
— ID 24.2 25 25.3 60 24.2
o 26.1 30 25.1 80 23.5
10 25.9 40 24.7 100 23
Solubility op Lithium-Potassium Sulfate in Water.
(Spielrein, 19x3.)
Gms. per xoo cc. Gms. per xoo ec.
*•• Sat, Sol. Solid Phase. f. |Sst, Sol. SoUd Phase. '
LiiSO*. K,S04. LI,S04. K,S04.
20 35. 6 3.6 LisSOi-KiSOi+LisSOi 60 10.6 16.3 LltS04.KfS04+K|S04
20 13.3 13. 1 " 4-K,S04 98 30.2 9.3 " -hLijS04
60 32. s 6 " +Li|S04 98 9 33 " +KfSp4
Sco^ubility op Lithium-Sodium Sulfates in Water,
(Spielrein, 19x5.)
Gms. per xoo oc. Gms. per xoo cc.
f. Sat, Sol. Solid Phase. y. Sat., Sol. . Solid Phaia.
LitSOf. NaaS04. Li«S04. Ns^fiOt.
o 31.4 5-9 Li,S04.Na,S04.5lH,0+Ll,S0« 33.5 25.8 i3.9L^S04.Na,S04.3lV)4-Ll,S04
o 18.5 11.4 « "+Na,S04 33-5 13-9 21 8 " +Ns,S04
7.5 20.4 II. 17 « (triple pt.) S3 28 166 " +LI,S04
16 32 9.3 " " S3 16.7 27.3 " +Na,.S04
34 26 14.9 Li,S04.Na«S04.xaH«0+Li,S04 99 27.4 14.4 " +L1,.S04
34 16. S 21.4 « +Na,S04 99 14.4 25.1 " +NS.SO4
32 20 16.8 " (triple PC.)
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, X910.)
10 cc. sat. solution in abs. H1SO4 contain 2.719 gms. LUSO% and the crystalline
solid phase has the composition LisS04.7HiS04 and melts at about la"*.
LITHIUM SULFATE 378
Solubility of LiTmuic Sulf'atb in Aq- ll^SOi at 30^ (vaa Doip, 191a)
Gms. ptr zoo Cms. Sat. SoL „ t> • «»l Gdm. per xoo Cms. Sat. Sol. «. v^ m^
t ■ * » Solid Phase. , * » Solid Phaie.
HiSO«. Li«SO«. o««i^n«. H«S04. Li|SO«. ^-m*^™*-
5.05 22.74 LisS04.HiO 55 08 13-69 LiS04
12.23 20.45 " 61.46 17.10 "
16.60 19.10 '^ 62.49 18.89 L]tS04.HiiS04
32.70 13.37 " 69.40 13.7s "
42.98 10.57 " 78.23 11.64 "
52.72 11.44 " 83.43 1565 "
Solubility of Lithium Sulfate in Aqueous Alcohol at 30^
(Sdueinemakezs and van Dorp, Jr., 1906.)
Gms. per xoo Cms. Sat. Sol. _ ,. . ^. Cms. per xoo Gms. Sat. Sol. _ ,..«..
4 »^ > Solid Phase. / * > Solid Phaae.
CAOH. Li,S04. *»»««^n«. c^^H. LiiSO*. «« i^-^.
o 25.1 LisS04.H^ 47.28 3.04 L]tS04.H/)
11.75 16.16 " 5&-59 1-22 "
21.19 "52 " 69.39 0-396 "
^29.40 8.17 " 80.74 o "
3.31 6.66 " 94-11 o "
I
'.•pt. data for LisS04 + MnSOi are given by Calcagni and Marotta, 1914:
Results for LisSOi + SrSOi are given by Calcagni and Marotta, 191 2. Results
for LiiSOi + NasSOt and LisSOi + KtSOt are given by Nacken, 1907; results for
LiaSOi + AgsSOi are given by Nacken, 1907b.
SILICATE LisSiO,.
Fusion point data for LitO + SiOt and LisSiOt -H ZnSiQt are given by van
Klooster, 1910-11. Results for LisSiOi + MgSiOs, LiiSiOi + NasSiOt, LiiSiOt +
KsSiOs and LiiSiOi + SrSiOt are given by V^llace, 1909.
UTHIXJM TABTEAT18.
Solubility in Water.
Gms. Salt
Salt. FMmula. t*. periooGmt. Authority.
Sat Sol.
Lithium Dihydioxytartratb LisC4H40s.2|HsO o 0.079 (Fenton, 1898.)
Lithium Sodium Racemic Tartrate LiNaC«H40».2HsO 30 IQ.97 (Schkasberg, 1900.)
" " Dextro " " 20 22.55 "
'' Potassium Racemic " LiKC4H406.HsO 20 35.19 '<
" " Dextro " " 20 37.82
MAQMKSIUM Mg. F.-pt. data for Mg+Hg. (Cambi and Spetoni. 19x5.)
MAGNESIUM ACBTATl Mg(CH,COO)s.4HsO.
Equilibrium in the System Magnesium Oxide-Acbtic Acid-Water at 25°.
(Iwaki, 19x4.)
Gms. per 100 Gms. Gms. per zoo Gms.
Sat.SoL Solid Phase. Sat. Sol.
CHiCOOH. MgO. CHiCOOH.
3.36 1. 73 MgO 31.37
5.65 2.93 " 36.23
8.06 4.21 « 35.77
12.46 6.54 " 40.87
1 5 . 46 8 . 24 " +(CHtCOO)sUg.4H«o 47 . 86
15-38 8.31 (CH«C00)tMg4H^ 56.16
14.25 7.24 « 61.59
20.19 7-47 " 69-13
22.93 7.60 « 75.93
26.61 7.74 " 82.90
2.3.3 = 2(CHjCOO)tMg.3CHtCOOH.3H20. More careful work in the renon
of the double salt showed that a second double salt of the composition 5(CHtC00)s
Mg.10CHtCOOH.7HsO was obtained. This compound usually separated from
the more concentrated acetic acid solutions.
Solid Phase.
MgO.
7.99(CH,COO),Mg.4HiO
8.18
+
8.17
s^.3
7.42
M
6.74
M
5.81
M
4.68
M
3-7S
M
2.85
«
2.23
•
579 HAGNESIUM BKNZOATE
MAQinsnTM BENZOATE Mg (CeH4COO)t.4H,0>
loo gnis. HiO dissolve 6.16 gms. Mg(C«HtCOO)t at 15° and 19.6 gms. at loo^
(Tarugi and Cheochi, 1901.)
100 gms. H«0 dissolve 3.^ gms. Mg(C6HiC00)t at 15-20. (Squire.and Caincs, 1905.)
MAaVESIUM BROMATX Mg(BrO,)>.6H,0.
100 cc. sat. solution contain 42 grams Mg(BrOs)„ or 0.15 gram mols.
at IS**.
(KaUraasch — SiUb. K. Akad. Wias. (BcriliOi U 90. '97^
MAaVBSIITM BROMIDE MgBr,.6H,0.
Solubility in Water.
(MenKhntUn — Chem. Centrb. 77t !• 646, '06; at 18*, Myliua and Fuok ^ Ber. 30b I7x8» '97 •)
«•
Gxaras MgBi> per xoo Gms.
SoludoQ. Water.
f. '
>ramaMgBrsj
^r 100 Gru
%
Solution.
Water:
— 10
47.2 89.4
40
50.4
IOI.6
0
47.9 91.9
SO
51.0
104. 1
10
48.6 94.S
60
SiS
107. s
18
49.0 96.1
80
53-2
113 -7
18
50 . 8 103 . 4 (M. and F.)
100
54-6
120.2
20
49.1 96.5
120
56.0
"75
25
49.4 97.6
140
58 0
138-1
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
wrhicb are evidently too high.
MAQMESIUM BROMIDE ETHERATES, ALCOHOLATE8, ACIDATES,
ETO.
SoLUBiLiTiBS Rbspbctively IN Ethbr, Alcohol, Acids, Etc., at
Various Temperatures.
(Boris N. Menachutkin. Monogratdi in the Russian lan^age entitled " On Etheiates and Other M<4eo-
tilar Combinations of Magnesium Bromide and Iodide." St. Petersburg, 1907, pp. 267 and XLVIII.
Abo pobHshed in the Memoirs of the St. Petersburg Polytechnic Institute, Vols. 1-7, X904-X907, and
in condensed fonn in Vols. 49-62 of the Zeit. anorg. Chem., 1906-1909.)
Preparation of Material. The dietherate of magnesium bromide,
MgBrs.2(CiHi)tO (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, MgBri.CCsHOsO, 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 ligrdin.
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 BBOMIDE
BTHERATBS
380
Solubility of Magnesium Bromide Dietherate, MgBrt.2(CtHfi)sO, and of
Magnesium Bromide Etherate, MgBrs(CsHt)tO, in Ethyl Ether, (CtHs)iO,
AT Various Temperatures.
Solubility of the Dietherate
Solubility of the Monoetherate
in
Ether.
in Ether.
r.
Cms. per xoo Gnu. Sat. Sol.
i;fgBrt.2(C,H|)«0. MgBr,.'
Mols. McBrt.
aCCH^iO per
xoo Mols.
Sat. SoL
r.
„ „ » « . Mol».MiBr»
Gnu. per 100 Gnu. Sat. SoL (CJUiO per
- 8
1.08
0.6
0.24
0
68.8
49.1 28.1
0
1.44
0.8
0.32
20
67.2
47
9 27.1
+10
2.3
1.27
0.52
30
66-5
47
3 26.6
14
2.9s
1.64
0.67
40
65 -5
46.
7 26.1
16
3.48
1-93
0.80
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
1. 125
100
60.7
43
3 23.5
22.
8 6.3
35
1.6
120
59-6
42
5 22.9
Two liquid layers separate between these con-
140
58.5
41
7 22.3
•
oentzations of MgBrt.a(C|H«) A
158
57-5
41 21.9
23
72.3
40.1
36.8
Two liquid layers separate between these oon-
24
75 -3
41.8
40.5
(
centntioBS ci MgBi|.(CH|} A
26
795
44.1
46.6
158
5-8
4.15 1.6
38.
s 84.2
46.7
54-2
158
4.8
3-4 1-36
30
85.5
47-4
56.9
159
162
1.96
0.38
1.4 0.56
0.27 O.II
170
0.18
0
.13 005
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.
Gnu. per
XOO Gms. Solution.
f.
r
Lower Layer.
Upper Layer
»
MgBrr2(CiHi)iO.
MgBr»
UgBcMCCIUiO.
MgBr,
— 10
75-75
42
3-2
1.8
0
73-9
41
4.1
2-3
+10
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
51
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. IS
9.2
5-1
158
74
41
7.8
4-3
unstable
«
it
stable
381
MAGNESIUM BBOMIDE
ALCOHOLATBS
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
MKBr,.6CH<0H MgBr,.6C,H|0H MgBr,.6CiH70H MgBr,.6 IS0C4H9OH
in Methyl Alcohol. in Ethyl, Alcohol, in rropyl Alcohol, in IsoButyl Alcohol.
*•.
Gins. MgBrs.
6CH1OH
!•.
Gms. MgBrt.
6CH»0H
t*.
Gms. MgBrs.
6CsH,OH
t*
Gms. MgBrs.
6C«H|0H
w •
per 100
V •
per xoo
w ■
per
100
V •
per 100
Gxna. Sat. Sol.
Gms. Sat. Sol.
Gms. Sat. Sol.
Gms. Sat. Sol.
0
42.6
0
17.2
0
77.9
0
SS.8
20
44.6
10
24.9
10
81.
S
10
60.5
40
46.7
20
32.7
20
8S
I
20
65.2
60
48.9
30
40.3
30
88.
5
30
69.8
80
SI. 4
40
47.8
40
92
40
74-3
100
55-5
60
62.2
43
93
SO
78. s
120
60.7
80
73.8
46
94.3
60
82.4
140
66.8
90
78.7
48
9S
8
6S
84.2
160
74
100
86.7
SO
97-
8
71
88
180
84. 5
103
90
52m.pt. 100
75
92
I8S
88
106
94.4
77
94.6
1901n.pt. 100
108. s
m.pt. 100
80 m.
pt. 100
i
1
Solubility of
Solubilit
y of
Solubility of
MgB
rs.6 Iso CtHuOH
MgBr,.4(CH,
,),CHOH
Mg
infi
Br,.4(CH,),C0H
in IsoAmyl Alcohol.
in Dimethyl Carbinol.
imethyl Carbinol.
f.
Gms. MgBrs.
6CiHuraper
Gm
*. 4(C]
* • per
s. MgBrs.
ai),CH0H
f.
Gms. MgBif.
4(rH,),C0H
zoo Gms.
100 Gms.
per zoo Gms.
Sat. Sol.
1
Sat. Sol.
Sat. Sol.
0
70.2
0
40
24. 7 m. pt. of (CH|)|C0H
10
75-6
20
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
100
59
55
32.2
40
90
120
67.3
60
40.5
42
92
130
74
70
62. s
44
94.2
136
83.6
75
77
46 m. pt. 100
138
90
79
91.5
139 m. pt.
100
80]
n. pt.
100
MAGNESIUM BBOMIDB ANILINATBS.
Solubility of Magnesium Bromide Anilinates in Aniline at
Different Temperatures. (Menschutkin, Z907.)
The compounds were formed by the action of aniline on magnesium bromide
dietherate. The three compounds were: MgBri.6C6HtNHs, MgBrt.4C6H4NHi
and MgBrt.2CeH5NHs.
t".
Gms. MgBrs.
per zoo Gms.
Sat. Sol.
Solid Phase.
f.
Gms. MgBrs.
4CW?Hs
per zoo Gms.
Sat. Sol.
Solid Phase.
10
3.2
MgBr^6C|HftNU|
160
26
HgBrMCANUt
50
5.1
11
180
28.3
If
70
7.5
w
200
33.5
u
90
12.8
M
220
45
tt
100
18. 5
U
230
55
f(
103.5
27.5
u
237 tr.
pt
76.3
u
103 tr. pt.
24
MgBrs.4CANH^
250
77.3
MgBi^aCiHaNHs
120
24.3
M
260
78.1
«
140
24.3
«
270
79
«
MAGNESIUM BBOMIDI d8a
MAONSSIUM BBOMIDI FHKNYLHTDRAZmATBS.
Solubility of Magnesium Bromide. Phbnylhydrazinatbs in Phenyl-
hydrazine.
(Menschutkin, 1907.)
(Approziinate determinations.)
♦. 6C|H»NED«IH| Solid Phase. t*. 6C»H«NHNH;i Solid Phwc.
Sat. Sol. Sat. Sol.
20 3 M«Bri.6C«HiNHNa IOOtr.pt. $4.8 MsBxk^CANHJmg
40 7 " 140 60.8
60 16.4 " 180 68.4
80 33 - 200 73.4
99 54.8
MAONE8IUM BBOMIDB COMPOUNDS with Benzaldehydeand with Acetone-
Solubility Respectively in Benzaldehydb and in Acetones.
(McDschutkin, 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 MgBr,.3CeH,C0H SolubUity of MeBr,.3CH,.C0.CHf.
in Benzaldehyde. in Acetone.
u
M
r.
Gms. MffRrt.
3r*H,COH
per xooGms.
Sat.SoL
r.
Gxna. MgBh.
3r«H,COH
per xooGms.
Sat. Sol.
f.
Gms. MgBiji.
3CHa.C0.CH«
per xooGms.
Sat. Sol.
f.
Gms. MgBft.
3CH«COCH«
per xooGms.
Sat.SoL
0
0.7
140
17.8
0
• 0.2
75
SO
30
60
100
1-3
1.9
3-4
145
146
148
37. S
65
84.5
30
60
70
6.8
1-45
2
76
80
84
71.6
83 -3
89.8
120
6
153
93-2
73
55
88
95-2
130
95
159m.pt.
100
74
14
92 m.
pt. 100
MAONS8IUM BBOMIDB COMPOUNDS with Methylal, Ortho Ethylformate,
Formic Add and Acetic Acid.
(Menschutkin, 1907a.)
The compounds were prepared by the action of methybl, 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 hygroacopicity.
Solubility of Solubility of Solubility of Solubility of
MgBrt.2CH,(0CH,), MeBr,.2CH(0C,H»), MgBr,.6HC(X)H MpBr,.6CH,CC)0H
in Methylal. inOrthoethylformate
. in
Formic Add.
m Acetic Acid.
Gms. MgBr*.
«• 3CH,(OCH0t
^' per 100 Gms.
t".
Gms. MgBr..
3Cfl(OC|I^«
per too Gms.
r.
Gms. MgBrt.
6HC00H
per xooGms.
r.
Gms. MgBiw
6CH.CO0H
per 100 Gms.
Sat. Sd.
Sat. Sol.
Sat Sol.
Sat Sol.
30 0.3
0
II. I
0
49.8
17
0.3
40 0.4s
20
"S
20
57. 5
30
IS
60 0.6
40
14.8
40
65.1
50
4.5
80 0.7S
60
18.6
60
731
60
7.9 ^
100 0.9
80
25.7
70
78.1
70
16.2
106 I.I
90
35
80
86
80
38. S
2 liquid layers here
95
41
86
95
90
57-7
106 86.2
100
SO
88]
n. pt 100
100
71.8
108 90.8
los
66
los
80
no 95-4
no
88.5
no
89. 5
112 m. pt 100
II.4 m.
pt 100
112 m.
pt 100
383
MAGNESIUM BROMDMS
MAGNESIUM BBOMIDB COMPOUNDS with Acetamide, Acetanilide and
Acetic Anhydride. (Menachutkin. 1909.)
The compounds were prepared by reaction with magnesium bromide dietherate.
Solubility of
MgBr,.6CH,C0NH,
in Acetamide.
Gois.
t*. CONE^ Solid Phaae.
per zoo Gms.
Sat. Sol.
8am.ptolCHsCX3NHg CH|CONH|
Solubility of Solubility of
MgBr,.6CH,C0NHCtHi MgBr,.6(CH,C0),0
in Acetanilide. in Acetic Anhydride.
t".
80
3-1
70
21.7
60
40
so. 5*
S6
70
57.8
90
60.5
110
65
130
71. S
ISO
80
160
8S
165^
90
i69t
100
u
•1
(1
XI2
1 10
108
Gnu.
;Br,.6C
Solid Phase,
per 100 Gma.
Sat. Sol.
m. pt. oC CH^CX>NHCA
3-7
7.7
CHsCONHCA
It
CHiCONHt+MgBfs.-
CH«CONH|
HgBrt.CHcCONH«
107. S* 9
K
U
II
M
(t
M
120
140
160
180
200
205
307
209
13. I
193
25. s
35 3
59. S
73-2
82.5
loof
o
ao
40
"+MgBr,CHr 60
CONHCiHt 80
HgBr|.CH;CONHCA zoo
120
130
133
X3S ^
136.5!
M
•f
If
M
•I
Gms.
MgBrt.
t*. 6(CHiCOO)iO
per 100 Gma.
Sat. SoL
36.4
38.7
31.6
357
41. 1
48.4
57.8
69.8
77
85
100
«
* Eutec.
tm.pt.
MAGNESIUM BBOMIDB COMPOUNDS with Urethan aAd with Urea.
(Menachutkin* 1909.)
Solubility of Magnesium Bromide
Uredian Compounds in Urethan.
Gms.
4.. "'^Xfja"*^
Solid Phaae.
per xoo Gms.
Sat. Sol.
49 m.pt. of urethan
CiHiOCONHg
45 18.5
n
39^ 36.5
(1
35* 43-3
" +MgBr,.6CHdOCX>NH,
50 45.6 ]
MgBr,.6CA0C0NH.
70 51.3
M
80 56.2
II
90 66.5
«
915 75.5
l<
9it 69.4
" +MgBiMCiH/XX)NHt
100 73.8
MgBrMCiHiOCONH.
no 80
M
115 84.1
It
I90 90
II
133 100
II
Solid Phaae.
Solubility of Magnesium Bromide
Urea Compounds in Urea.
Gms.
per zoo Gms.
Sat. Sol.
132 m. pt. ci vna
136
120
114
108.5*
COCNHJ,
9 5
17.3
21.8
24. 2 C0(NH^,+MgBri.6C0(NQ^
u
<i
II
"5
120
127
130
i3ot
145
160
i6s
170
171
Eutec.
29.8
35
45.5
60
58
60.7
67.3
71.4
83.7
96
ttr.pt.
MgBrs.6C0<NHJt
11
M
II
<l
+MgBrs.4C0(NH^t
MgBr|.4C0(N^
(I
If
II
MAGNESIUM CAMPHOBATB CioHi«04Mg.i4HaO.
Solubility of Magnesium Camphoratb in d Camphoric Acid at 15^
AND Vice Versa.
(jungfleiach and Landrieu, 19Z4.)
' ^"T ' ^ „^u SoKd Phaae.
CnHm04. CuHmOa^.
0.622 (13.5V 0 CioHu04
1 . 20 1 . 29 **
1.98 3.53 ;;
3.|6 5.66
3.85 8.19 "
CuHi«04.
3.16
3-5
3.6
1. 91
0
CioHi404Mg.
10.30
16. 5
16.7
15. 1
14.35
Solid Phaae.
CioHu04
" -|-CioHH04Mg.i4H,0
CioHt404Mg.i4HsO
«
MAGNSSIUM CABBONATK 384
MAGNESIUM CABBONATB MgC0s.3HA
Solubility in Water in Prbsbncb op Carbon Dioxidb at ij®.
Cneadwell and Reuter — Z. anorg. Ch. 17, 900, 'g8.)
Oijperioooc.
1 Pbase (at oP
d 760 mm.).
Partial
PRnure of CO)
in mm. Hg.
Grams per
xoo oc. Solntian.
'^Ftee COj.
MgCOft.
Mg(HCOj),.
Total Mg.
18.86
143 -3
O.II90
• • •
I. 2105
0 . 2016
5-47
41.6
0.0866
• • •
I. 2105
0 . 2016
4-47
33-8
00035
• • •
I. 2105
0.2016
1-54
11.7
•>■ •
0.0773
1.0766
0.2016
1-35
10.3
0.0765
0.7629
0.1492
1.07
8.3
0.0807
05952
01224
0.62
4-7
0.0701
03663
0.0865
0.60
4.6
0.0758
0.3417
0.0788
0 33
2-S
0.0748
0 ■ 2632
0.065s
0.21
1.6
0.0771
0.2229
0.0594
0.14
I.I
0.0710
0.2169
0.0566
0.03
03
O.071I
0 . 2036
0.0545
• • •
• • ■
00685
0 . 2033
0.0536
• • •
• • •
00702
01960
0.0529
• • •
• • •
■
0.0625
0 . 2036
0.0520
• • •
• • •
00616
0.1954
O.051I
• m 9
• • •
0.0641
0.1954
0.0518
Therefore at o partial pressure of COi and at 15* and mean barometric pressure,
one liter of saturated aqueous solution contains 0.641 gm. of MgCOi plus 1.954
gms. Mg(HCO,)j.
It is ^inted out by Johnston' (19 15) 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 of Magnesium Carbonate in Water Charged with Car-
bon Dioxide at Pressures Greater than One Atmosphere.
(Engel and Ville — Compt. rcnd. 93, 340. '8x; Engel — Ann. chim. phys. [6] 13, 349, '88.)
P«««««of G. MrCOs* per LitPT. ^^fS^^ ^ G. MgCOa* per liter.
CO2 in /r " a > CO2 m t . *:: . h
Atmospheres. At ia°. At xp**. Atmospheies. At 12*. At 19*.
0'5 20 '5 ••• 4-0 4^'^ ***
i.o 26.5 25.8 4.7 ... 43.5
20 34.2 33.1 (2.1 At) 6.0 50.6 48.5 (6.2 At.)
3.0 390 37.2 (3.2 At.) 9.0 ... 56.6
Solubility in Water Saturated with CO, at One atmosphbrb.
(Engd.)
*«».
Gms. MgCO^
per liter.
t».
Gms. MgCO^
per liter.
t».
Gms. MgCO^
per liter.
5
36
30
21
60
II
10
31
40
17
80
5
90
26
100
0
Dissolved as Mg(HCOs)t.
385
MAGKUIUM CABBONATB
Data for the system magnesium carbonate-carbonic acid- water at 20^, 25^ 30^
^^ and 39^ are given by Leather and Sen (19 14). In connection -vith these results,
It is pointed out bv Johnston (19 15), that it is questionable whether eauilibrium
was really obtained and furthermore, the accuracy of the analytical results cannot
be trusted since the ratio of tokU amount of COt in solution, to the magnesia la
very irregular. The results when plotted directly show great inconsistencies.
The Calculated Solubility of MgCOi.3HiO in Water at 18® in Contacd
WITH Air Containing Partial Pressures of COi from 0.0002 to 0.0005
Atmospheres.
(Johnston, 1915.)
It is shown that if the COi 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)t or of MgCOi.3HsO will be obtained.
Partial Preasure P
of COk in Atma.
O
0.00020
0.00025
0.00030
0.0003s
0.00040
0.00045
0.00050
Solubility of
Total Mg
Mols.
/
0.00015
0.01934
0.02218
0.02486
0.02742
0.02868
0.02924
Cms. per Liter.
0.0087 Mg(OH)i
1.29
I -45
1.60
3-97
4.05
1.12
IN Natural Waters.
It
tt
u
((
MgCCsHiO
«
((
0.02976
Magnesium Carbonate
(Wells, 19x5.)
(In all cases the solutions were in equilibrium with atmosoheric air at 20^.)
MUlignuns per Liter of Sat. Solution.
Mixture.
Mg.
0.018
0.028
FreeCO^.
trace
trace
CaasBi-
carbooate.
0.065
0.086
Natural Magnesite in Distilled HsO
" in Aq. NaCl (27.2 g. per 1.)
MgCO|.3HsO (equilibrium from bicarbonate end) 0.038 0.28 COs as carbonate 0.83
MgCO».3HiO( " " under saturation ") 0.034 0.32 COi" " 0.59
Solubility of Magnesium Carbonate in Aqueous Solutions of
Potassium Bicarbonate.
(Aueibach, 1904.)
The conditions necessary for preventing changes in equilibrium due to hy-
drolysis and loss of COt ^re discu^ed. The mixtures were shaken from 1-4 days.
The sat. sol. analyzed for total alkali I K H J by titration with standard HCl
using methyl orange as indicator. The neutralized solution was boiled to expel
COi and then excess o.i n NaOH added and the filtrate from magnesium precipi-
tate back titrated with o.i n HCl. The ^
2
NaOH and the K obtained by difference.
was calculated from the used cm
Results at 15"*.
Mols. per Liter. _ ,. . ^.
i,„^^ ,, ^^ * Solid Phase.
KHCOb. MgCOb.
SoUd Phase.
Results at 35
Mols. per Liter,
EhcoT
O
0.0992
0.1943
0.3992
0.2681
0.5243
0.6792
0.981
z.x ■
0.0095 MgC0k.3H/)
It
tt
"(UbO)
« +X.X
0.0131
0.0167
0.02 1 1
0.0192
0.0097
0.0074
0.0028
MgC0^.KHC0^.4Hs0.
fi
II
II
z.x
14
II
" (Ubfl)
" +X.X
x.x
II
II
o
0.1092
0.281 1
0.4847
0.5807
MgCOk.
0.0071
0.0098
0.0142
0.0177
0.0198
SoUd Phase.
MgCXV.3H^
II
II
II
Results at 25
Mob, per Liter.
£HC0k MgCOki
O 0.0087 MgC0k.3H/)
0.0985 0.01 1 5
0.2210 0.0149
0-3434 O.0181
0.4985 0.0217
0.3906 0.0196
0*5893 0.0128
0.6406 0.0117
1. 125 0.0061
Additional data for this system are given by Nanty, 191 1.
Data for the solubility of MgCOt 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 Gotne (1915).
0.5088 0.0184
0.6231 0.0153
0-8535 0.01 19
+X.X
«
X.Z
M
MAGNESIUM CABBONATK
386
Solubility op Magnesium Carbonate in Aqueous Solutions op
Sodium Carbonate at 25^. The solutions being in eqtiilibrium
with an atmosphere free from CO,.
H^t. of I Liter
Crams per
Liter.
Reacting Weights per Liter.
of Soludoa.
Ka^O*.
Mgcx)*:
'Na^Oi.
Mffco*:
996.8
0.00
0.223
0.000
0.00266
IOI9.9
23.12
0.288
0.220
0.00344
1047.7
50-75
0.510
0.483
0.00620
1082.5
86.42
0.879
0.820
0.01027
II18.9
"7-3
1-314
1.209
0.01570
II47.7
160.8
1.636
1.526
0.0195s
I166.I
181 .9
1.972
1.727
0.02357
I189.4
213.2
2.317
2.024
0.02770
Solubility op Magnesium Bi Carbonate and op Magnesium Car-
bonate IN Aqueous Solutions op Sodium Chloride at 23°. The
solutions being in equilibritim with an atmosphere of COs in the
one case, and in eqtulibrium with air free from CO, in the other.
(C. Md s.)
In Presence of COt as Gas Phase.
0ms. NaQ
per Liter.
Cms. Ms(HCQi)a
per Liter.
7.0
30.64
56.5
30.18
119. 7
27.88
163.9
24.96
224.8
20.78
306.6
10.75
Wt.of I
Liter.
996.9
IO16.8
I04I . I
1070.5
1094.5
1142.5
II70.I
"99-3
In Presence of Air Free from CO».
Gms. NaQ
per liter.
0.0
28.0
59-5
106.3
147.4
231.1
272.9
331-4
Gms. MjrCOk
per Liter.
0.176
0.418
0.527
0-585
C.544
0.460
0.393
0.293
Solubility op Magnesium Carbonate in Aqueous Solutions of
Sodium Sulphate at 24° and at 35.5°. The solutions being in
eqtulibritim with an atmosphere free from CO,.
(Cameraa and Seidell.)
Results at 24^
Wt.of
Gms. Na^SO^
Gms. MgCOi
z Liter.
per liter.
007-5
o.oa
0.216
I02I.2
25.12
0.586
1047.6
54.76
0.828
1080.9
95-68
1.020
"33-8
160.8
1.230
"57-3
191.9
1.280
1206.0
254.6
I 338
1242.0
305 I
I.3S8
Results at 35.5.
Wt.of
I Liter.
Gms. NagSQi C
per Liter.
995 I
1032.9
1067.2
1094.8
1120.4
"51-7
0.32
41.84
81.84
116.56
148.56
186.7
1179.8
224.0
1236.5
299.2
per Liter.
O.I3I
0.577
0.753
0.904
0.962
1.047
1.088
I 130
lUaMUIUH CHLOBATI
BUOmSIUM CHI.OBATK Mg(CI0.)..6H,0.
Solubility in Water.
laOTi-imaaj,
SclulkB.
>I^
'So
-l8
51.64
10
OS
o
S3 "7
10
73
tS
56.50
13
33
60.33
14
35
3S
63.65
16
48
to ifi(aoi)i
Hi<CIOdi SoBd.
■^iss-
ȣS.'So. "^
43 63 -Sa
16.60 Hi(CIOi)»4H.O
65.5 69. »
20.08
39 S 6S 37
17.76 uccacwwHiO
61.0 69.46
al.40
68 70.69
aa.69
93 (73-70
{26. 3S) -
» - 1.564.
Sp. Gr. of saturated sol. at + 18°
H4ainSIUH OHLOaiDB MgCl,.
SoLUBiLiTy IN Water.
(Tin'tHdlaiidMcTertuiffH, iSjA Engil; Lomnbsi. RcBi]liqiiatcdEniaiI«BiliiltuidB<InMbia,iBtt.)
.. G™.M»n
■"■"O"
SgHd
. . Gnu. MeC
,p«,«
Gmi-SoBd
* ■ gohuioa.
wSS.
Phut
*' ^^hlU^
»»>.
— 10 II.I
"■5
In
0 34-5
sal'
Uga».6B.o
— ao 16.0
19.0
"
10 34-9
53-5
••
-30 19.4
34 -0
"
ao 3S -3
S4-S
"
-33.6 ao.6
a6.o
i«+Mga,.t
.HK> aa 35.6
SS-*
— ao 36.7
36 s
H(CI|.i)H,0
as 36-a
S6-7
"
—16.4 30.6
44 -04 '-[«-. "
40 36-5
57-5
■ "
-16.8 31.6
46.3
M
60 37.9
61.0
"
-17-4 323
47 ft*
U
80 39.8
66.0
"
100 43.3
73 0
-19-4 33-3
- 9-6 33-9
49-9*
CT I*
M
116.7 46 a
8S-S
!"«»■.*
51-3
U
iSa.6 49 »
96.4
Mga,.»H,0
-3-4 34-4
5a -3
•boiiii8i.5 S5-8 136.0
i"efi«i
186 56 . 1
138 .0
M«CIt.H,0
80LUBILITT OF Maonbsiuh Chloride in Aquboits SoLtmotts of
Hydrochloric Acid at o".
(Engd — Ccaj^. raid. 104, U3, V7J
•^15:
,U^, ■ SH.^.
■ aa.
MKfc-
0.0
99.55 1.363
0.0
474.3
4.095
95 S 1354
■493
454.8
9S
90.0 1.344
34.63
438.6
17.0
83.5 1.300
61 97
393 0
30.5
79.0 1.397
74-74
376.3
38.5
71.0 1.381
103.9
338.3
43.0
60.135
153."
,86.4
58 75
46.35
314.3
330.3
J6.0
33.0
377.1
153.0
at. HCl (Ditle)
6.5
0 gms. H«0 dinolve 53.65 gnw. Mgdi at 3.5°, 55.36
glM.
at 35° and 5S.66
«50°.
aataiMVuaM.mti
MAGNESIUM CHLORIDB 388
Solubility of Basic Magnesium Chloride in Water at 25^
(Robinaon and Wasgamaa, 1909.)
An excess of MgO was shaken with each of 20 MgClt 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 HCl for dissolved MgO
(present as Mg(OH)s). The composition of the solid phase in each case was
ascertained by plotting the analytical results on a triangular diagram.
Gms. per zoo Gms. , , Gms. per 100 Gms.
Sat. Sol.
^
t. Sol
Solid Phase.'
d»oi
Sat. Sol.
.Sol.
Solid Phase.
MgCl,.
MgO.
MgCl,.
MgO.
1. 019
2.36
0.00008
Indefinite
1. 141
17.53
0.0024
2MgO.HCl.5HiO
1.038
4.47
0.00028
Solid Solution
1. 162
18.52
0.0025
«
1.056
6.79
0.00048
{<
1. 192
22.04
0.00245
«
X.07S
9.02
0.00080
tt
1.245
26.88
0.0025
«
J. Ill
13.14
0.00115
it
1.274
29.80
0.0024
«
1. 321
34.22
0.0030
, t€
Solubility of Mixtures of Magnesium Chloride, Potassium Chloride
and of Magnesium Potassium Chloride (Carnallitb) in Water at
Various Temperatures.
(van't Hoff and Meyerhoffer, 1899, 191a.)
Gms. per ico
f. Gms. H,0. Solid Phase. Kind of Pobt on Curve.'
MgCli. KCl.
— ii.x ... 24.6 Ice+^ia Cryohydric of KCl
-33.6 26 ... " +MgaMsH^ " MgCls.i2H|0
-34.3 22.7 1 . 24 " +Ka+MgCI,.iaH^ " " -hKa
— 21 34.9 2.o3CaniaIlite+MgClt.x3l^+KCl Formation Temp, of Camallite '
— o 35.5 3.02 " +Ka Point on Curve
25 38.4 4.76 "+"
50 42 6.17 " + " " " (UhUf,x9i3.)
61.5 42.6 7.20 " + '• " "
154. S 65.5 14.07 " + « " "
167 . 5 88 . 1 17 . 26 " + " M. pt. of Carnallite
25 55.5 0.83 " +Mgat.6H^ Point on Curve
50 59.13 0,50 "+ " " " (Uhlig, 19x3.)
80 65 1 . 24 " + " " "
1 15 . 7 85 . 6 1 . 66 " + " +MgClt.4H^ Transition Point [Carnallite
152.5 105.7 9.93 " +MgCl,.4H^+Ka Upper Formation Temp, of
1 76 1 26 . 9 16.97 MgCli.4H,04-MgCI«.2Hi0+Ka Transition Point
z86 126.9 26-1 MgCl«.2H^+Ka Point on Curve
Carnallite = MgKCU.6H,0.
Solubility of Mixtures of Magnesium Chloride and Other Salts in
Water at 25". ;
(LOwenherz, 1894.) «
MiztuK ^°^' ^^^' T^^ ^^*°^ Mols. H|0. Gms. per Liter of Solution.
MgClt.6H/)-|-MgS04.6HiO 104 MgCltH-i4 MgS04 25. CI-|-4.4 SO4
MgCl,.7HiO-fMgS04.6H,0 73 " +15 " 19.5 Cl-f 53 SO4
MgCli.6HiOH-MgClt.KC1.6H,0 106 Ot+i Kt+ios Mg 26.9 ClH-o.3 K-|-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. MgCU at room temp. A flocculant
ppt. separates on standing. ^ ^ (Welsh and Broderson, 19x5.)
Freezing-point data (solubility, see footnote, p. i) for mixtures of MgCls and
KCl, NaCl, AgCl, ZnCl* and SnCU are given by Menge (191 1). Data for mixtures
of MgClj + SrClj and MgClj -j- MhCU are given by Sandonnini (1912, 1914).
Data for MgClj 4- MgS04 are given by Jaenecke (191 2). Data for MgCU+TlCl
are given by Korreng (1914) and data for MgCla+KCl and MgCli+HCl aiegivea
by Demby (1918).
389
MAGNESIUM CINNAMATB
MAGNESIUM CINNAMATE (C«H«.CH.CH.C00)2Mg.HA
loo gms. sat. solution in water contain 0.85 gm. (C6HfiCH.CHC00)iMg at
15° and 1.94 gms. at IOO^ (Tarugi and Cbecchi. 1901.)
MAGNESIUM CHBOMATB MgCr(X.7HiO.
100 grams HtO dissolve 72.3 grams MgCr04 at i8^ or 100 grams solution con-
tain 42.0 grams. Sp. Gr. » 1422. (Mylius and Funk, Z897O
MAGNESIUM POTASSIUM OHBOMATE MgCr04.K,Cr04.2H,0.
100 grams H,0 dissolve 28.2 grams at 20^, and 34.3 grams at 60^.
(Sdiwditxer i)
MAGNESIUM PLATINIO OYANIDE MgPtCCN)^,
Solubility in Water.
Gms.MgPt(CN)«
Gms. MgPt(CN)k
t«.
per 100 Gms.
Sohation.
SoUd Phase.
t*.
per zoo Gms.
Solution*
RnlldPIiMe.
—4.12
24.90
MgPt(CN)«w6^8.iHsO
48.7
40.89
]&fl]tPt(CN>«^HsO
O-S
26.9
" (Red)
55
41.33
M
S'S
28.65
u
58.1
42.15
»
18.0
32.46
M
69.0
43-40
a
36.6
39 53
M
77.8
4490
«
45 0
41-33
U
87.4
45 -P
•i
46.2
42.0
M
90.0
45-65
M
42.3
40.21
MgPt(CN)4.4HsO
93 0
45-04
M
46.3
39 85
" (Bright Green)
96.4
44.33
MgPt(CN)«.aHaO
100. 0
44.0
(White)
MAGNESIUM FerroCTANIDES.
Solubility in Water at i7*.
(Robinson, 1909.)
One liter sat. sol. contains 1.95 gms. magnesium potassium ferrocyanide,
MgKjFeCN,.
One liter sat. sol. contains 2.48 gms. magnesium ammonium ferrocyanide,
Mg(NH4)»FeC,N,.
MAGNESIUM FLUORIDE MgF,.
One liter of water dissolves 0.076 gm. MgPt at 18° by conductivity method.
(Kohlrausch, 1905.)
One liter water dissolves 0.©87-o.09O gm. MgFi at 0.3** and 0.084 K™. ^^ 27
by conductivity method. (Kohlntusch, 1908.)
MAGNESIUM HYDROXIDE Mg(OH)s.
One liter of water dissolves 0.008 — 0.009 gm. Mg(OH)i at 18° by conductivity
method. (Dupre and Brutus, 1903.)
One liter of water dissolves 0.009 g™. Mg(OH)j at 18" by conductivity method
(Kohlrausch and Rose, 1893), 0.012 gm. (Tamm, 191 o).
Solubility of Magnesium Oxide in Aqueous Solutions Containing
Sodium Chloride and Sodium Hydroxide.
(Maigrct, 1905.)
f«m« VaCI
Gms. MgO per Liter Solution with Added:
per liter.
'0.8 g. NaOH 40 g. NaOH"
per Liter. per Liter.
"5
0.07 0.03
140
0.045
160
none none
MAaNSSIUM HTDROZmS
390
Solubility op Magnesium Hydroxidb in Aqubous Solutions op
Ammonium Chloride and op Ammonium Nitrate at 29^.
(Hen and Mobs — Z. anois. Ch. 38^ 140^ '04.)
Note. — Pure M^(OH)a was prepared and an excess shaken with
solutions of ammonium chloride and of ammonium nitrate of diffefent
concentrations.
i^ n nmtr if ■■ m/ Acld RMIUind
lOW3flrolNH,NO.. t^ASf^^,
(Ncnn.1.) *™^2^T'
NonnaMtyoft
Mc(OH)9. NH^
•7
0.466
0-3S
0-3S
017s
(NH^d)
(NH4NO,)
M
o 09^35
0.II08
o 09^35
0.II08
0.II08
0.II08
0.II08
0.156 0.388
0.108 0.250 3.15
0.089 0.172 2.60
0.0638 0.106 1.86
0.049 0.0771 1.43
0.0833 o.i834(NH^o*)2.43
0.0495 0.076 ** 1.45
Mc(OH)|. NH«CL
4.55 20.86
13-39
9.21
5-67
413
i4.69(NH«NOi>
6.09 -
MAaHlSIUM lODATl Mg(IO0i.
Solubility in Water.
(Melius and Fonk — Bcr. yo, ijm, '97: Win. Abh. p. t. RdcfaanHalt 3, 44^1 '00.)
Gma.
Mob.
Gma. Mola.
f
Mg(IOfe),
pi^S^
Solid
t*
MgdO,),
Mgao,),^
Solid
w .
per 100
Phaae.
w .
per xoo
per 100 Mob.
Phaie.
Gma. Solution.
H,0.
Gma. Solution
. HsO.
0
31
0.15 MiaO^'ioHiO
0
6.8
0.34 M
tdO^A
20
10.2
O-SS
M
10
6.4
0.30
u
30
17.4
1. 01
M
18
7.6
0.40
M
35
21.9
I -35
M
20
7-7
0.40
«
SO
67 5
10. 0
M
35
8.9
0.47
M
63
12.6
0.69
M
100
19-3
113
M
Sp. Gr. of solution sat. at iS®*- 1.078.
MAGNESIUM IODIDE MgIt.8H/).
Solubility in Water. (Menschutkm. 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 determinaticms were made
by the synthetic method.
Gms. per zoo
Cms. Sat. Solution.
JL
SnIM Phftse.
MgI,.6H«0
- Mgl,.
0 76
547
Mgl2.8HiO
18
59.7 (rf-x.909)
" (MyliDsai
20 81
58.3
u
40 88
63.4
tt
43.5tr.pt. 90.8
65.4
" +MgI,.6HiO
43 898
64.7
MgIi.6H^
80 90.3
65
U
120 90.9
65.4
tt
160 91.7
66
tt
200 93.4
67.2
t€
215 94.3
67.9
tt
391 MAGNESIUM IODIDE
MAGNESIUM lODIDB BTHERATES, ALCOHOLATES, ACIDATES, etc.
Solubilities RESPEcrfvBLY in Ether, Alcohol and Acm Solvents at
Various Temperatures.
Boris N. Menachutkin. Monograph in the Ruasian Language entitled "On Etheratea and Other Molec-
ular Combinatbns of Magnwiiiiin Bromide and Iodide," St. Petersburg, 1907, pp. 367 + XLVIII.
Alao pubUshed in "Memoirs of the St. Petersburg Polytechnic Institute," vola. z-7, 1904-07 Lad in
oondenaed form in vols. 49-67 of the Zeit. aaoxg. Chem., x9o6-«9.
Projiaration of BCaterial. The dietherate of magnesium iodide, MgIi.2C4HioO,
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 aicohols, 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.
KzplAnation 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 MgIs.2C4HioO
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 MgIt.2(CsHt)iO; the temperature, 38.5^ At
concentrations of MgIs.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 lODIDl
392
Solubility' of Magnesium Iodide Dibtherate in Ether at Different
Temperatures. (Menschutkin, 2906.)
Gins, per loo Gms. Mols, MgI,.2(C^/>
___^ per 100 Mols.
S-4
II. 8
15.6
18. 1
20.4
22.2
23.6
.per
Sat.
MgI,.2(CA)^
2.2
3-7
8.3
II. 6
173
22
Sol.
Mgl,.
1-45
2.43
3 46
S-4
7.55
11.28
14.4
Sat. Sol.
0.39
0.66
0.96
i-SS
2.24
356
4.67
Solid Phase.
n
i<
u
u
u
a
Between these two concentrations of MgIi.2(CsHt)sO two liquid layers separate
below).
23.6
2S
30
35
40
45
Si.Sm.pt.
54. 4
73
82. s
87
89.6
93 S
100
35-5
47.6
54
57
58.6
61.2
65.2
17. 1
319
42.9
53-4
60.4
71.4
100
u
tt
ts
tt
tt
tt
At 23.6° the saturated solution separates into two liquid layers which have
the following composition at different temperatures.
Gms. per zoo Gms. Solution.
r.
15
20
25
30
35
36
37
38
Lower Layer.
MgIa.2(CsH«)^ - Mgl|.
54
54
54
54
54
53
52
50
38 . s crit. temp. 40
4
4
4
4
I
5
2
5
3
35
35
35
35
35
34
34
33
26
5
5
5
5
3
9
2
I
3
Ui
Mgl,.2
20.5
21.5
22. S
235
26
27
28. s
32
40.3
T Layer.
lO-Mgl,.
134
14. 1
14.7
15.4
17
17.7
18.7
21
26.3
unstable
ic
Stable
it
tt
(t
tt
it'
MAGNESIUM IODIDE ALCOHOLATBS and ANILINATB.
Solubility of Each in the Respective Alcohols or Aniline. (Mensdratidn.)
MgI,.6CH,0H
in Methyl Alcohol.
Gms.
^ Mgl3.6CH/)H
* ' per 100 Gms.
Sat. Sol.
o 49.6
20 S2-6
40 55. 3
60 58.8
80 60.6
100 63.3
120 66.2
140 69.5
160 73 . 2
180 77.1
200 81 . 5
MgI,.6C,H*0H
in Ethyl Alcohol.
Gms.
*• MgIt.6C|HtOH
per 100 Gms,
Sat. Sol.
Gms.
MgI,.6CANHa
per xoo Gms.
Sat. Sol.
O
20
40
60
80
100
120
130
140
143 ^
146. 5t
21
33
44
55
65
74
82
87
93
96
100
9
2
4
3
5
7
7
2
3
MgI,.6CeH*NH, MgI,.6(CH,),CH0H
in Aniline. in Dimethyl CarbinoL
Gms.
Mel«.6(CH,)r
CHOHper xoo
Gms. Sat. Sol.
57.1
60
63.3
67
71.2
76.2
79.4
84.8
91.7
100
o
60
100
130
150
170
180
i88t
200
210
230
3-3
3.9
5
8.5
17.5
38
52
64.5
65.9*
67.2*
69.8*
f.
10
30
50
70
90
no
120
130
136
i38t
• Solid Phase. MgI«.4CANH,. fM.pt. t Tlr.pt..
393
MAGNESIUM lODIDI
MAGNESIUM lODIDB COMPOUNDS.
Solubility of Magnesium Iodide Compounds with Bbnzaldbhydb,
Acetone, Acetal, and Acetic Acid in Each of these Liquids.
^Meoschutkin.)
Md[,.6C«H»C0H
in Benzaldehyde.
Gms. MgL.-
6CpH»C0H
per xoo Gms.
Sat. Sol.
r.
MgI,.6CH,COCH,
in Acetone.
Gms. MgL.-
eCHtCOCHi
per xoo Gms.
Sat. Sol.
O
20
40
60
80
100
IIO
120
"5
130
136
3-2
3.8
53
7.7
II
18.5
26.5
40
S3
74. 5
94.2
r.
o
30
50
60
70
80
8S
90
95
100
105
4.9
6.7
8.3
10.2
15.2
28.6
40
59-2
80
92.5
98.5
MgI,.2CH,CH-
(OCiHi)s in Acetal.
Gms. Mglf.-
^ aCH»CH(OC»Hi)s
* * per xoo Gms.
Sat. Sol.
20 0.15
60 0.45
77 0.60
(Between these two con-
centrations the mix-
tare separates into two
liquid layers.)
77 92
79 93-7
81 95-5
83 97-3
86m.pt. 100
MgIi.6CH,CqOH
in Acetic Acid.
Gms. Mglf.-
^ 6CH»COOH
per xoo Gms-
Sat. Sol.
20 ■ 0.6
40 2
60 s
70 9-5
80 18.5
95 42
105 54. 5
"5 6s
125 73-8
135 8s
140 94
142m.pt. 100
i39m.pt. 100 Io6.Sm-Pt- 100
^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.
(Menschutkm.)
MgI,.6HCOOC2H, MgI,.6CH,C0OCH, MgI,.6CH,C00C,H, MgI,.6CH,C0OCiHT
in Ethyl Formate, in Methyl Acetate. . in Ethyl Acetate. in Propyl Acetate.
r.
Gins. Mgl|.-
6HCOOC,H|
per 100 Gms.
Sat. Sol.
r.
Gms. McL.-
6CH»COOCHi
per xoo Gms.
Sat. Sol.
r.
Gms. MgL.-
ecHiCOorjH,
per x<» Gms.
Sat. Sol.
Gms. MgL.-
M 6CH|C00CtHf
per xoo Gms.
Sat. Sol.
0
15. 1
0
0.4
0
3-2
0 4.1
10
17 -4
60
0.75
20
4.8
20 S-4
20
20. s
90
0.9
40
8.6
30 6.5
30
25
100
1.8
SO
13-7
35 7.8
40
31-8
103
2.4
55
21.5
40 19
SO
44
(Two layers here.)
60
38
45 46
60
68
103
74.2
65
63 -5
SO 72.5
70.5=
in.pt. 100
IIO
81.7
70
90.5
55 88.2
120
98
75
92.7
60 96
I2Im.pt. 100
78.
Sm.pt. 100
6Sm.pt. 100
MgIs.6CH,COO (iso) C«H,
in Isobutyl Acetate.
MgIi.6CH,C00 (iso) C,Hu
in Isoamyl Acetate.
f.
Gms. MgIt.6CHr
coo (iso) C4H,
per 100 Gms. Sat. Sol.
Gms. MgI,.6CHr
f. [COO (iso) CHm
per 100 Gms. Sat. SoL
0
10. 5
0
7.7
20
13.6
20
"S
40
17.6
40
20.9
60
24.9
45
25. S
70
33-7
50
33-2
80
52
55
47.8
85
89
57.5
63
87.Sm.pl
••
100
60m.pt.
100
MAOMianJM lODIDl
394
Solubility of Magnesium Iodide Compounds with Acetonitrilb, Acbtamidb
AND UrETHAN in THESE LIQUIDS. (Menschutkin.)
MgIi.6CH,CN
in Aoetonitrile.
Gms. Mgl|.-
6CH,CNper
M^I,.6CH,C0NH,
in Acetamide.
f.
O
30
SO
70
75
80
8S
89
xoo Gms.
Sat. Sol.
37-2
49.8
58.2
67.9
71.7
76. S
83
91-3
f.
Gms. Mcl|.-
6CH,C0NHt
per 100 Gms.
Sat. Sol.
Solid PhsM.
MgI,.6NH,C(X)C,Hi
in Urethan.
Gms. KCglt.-
5Hi
82 m. pt. of acetamide
^ 6NH,C00
' per 100 Gms.
Sat. Sol.
49 ^"^ V^' o^ urethan
Solid Phase.
70
49*
80
130
160
170
i77t
28 CHsCONH^ 45
46.7 " 39
56.5 •+Mgl,.6CH,C0NH.32*
63.4 MgIi6CHsC0NHt 40
76 " 60
85.5 " 80
90.8 « 86
100
* Entec.
27.SNH1COOCA
45 "
51.8 "+MgI..NH,C00CA
55 MglfNHtCOOCA
64.7
78.8
925
100 ••
87t
t m. pt.
MAGNESIUM IODOMIBCU&4TB MgI,.2HgIs.7HiO.
The sat. solution in water at 17.8® has the composition MgIs.i.29HgIs.ii.o6HiO
and Sp. Gr. 2.92. (Duboin. 1906.)
MAGNSSIUM DiLACTATB Mg(C«HA).6H,0 racemic, Mg(C«HtO»).3HA
inactive.
Solubility of Racbmic and of Inactivb Magnesium Dilactatb in Water.
(Jungfleiscb, 191a.)
100 gms. HiO dissolve 7 to 8 gms. racemic and 2.28 gms. inactive lactate at 15^.
MAONSSIUM LAU&ATB, MTRI8TATB, PALMITATB and 8TKA&ATI.
Solubility of Each in Several Solvents. Qaoobeon and Hohnes, 19x6.)
Gms. Each Salt Determined Separately per xoo.Gms. Solvent.
Solvent.
f.
Mg Laurate
(c3LjC00)r
Mg Myriatate
Mff PahniUte
Mr Stearate
(CuSiCOO)r
«a*r
Water
IS
O.OIO
0.006
0.005
0.003
u
2S
0.007
0.006
0.008
0.004
it
35
0.010
0.007
0.006
0.007
u
50
0.026
0.014
0.009
0.008
Abs. Ethyl Alcohol 15
0.519
0.158
0.034
0.017
t(
25
0.591
0.236
0.058
0.023
u
35
0.805
0.373
0.085
0.031
t(
50
1.267
0.577
O.151
■ ■ •
Methyl Alcohol
15
I 095
0.571
0.227
0.084
«
25
1. 108
0.763
0.36
O.IOO
tt
Si-S
■ « •
• • •
0.50
0.166
Ether
25
0.015
O.OIO
0.004
0.003
Ethyl Acetate
IS
0.004
0.004
0.004
0.004
tt
35
O.OII
O.OIO
0.007
0.008
tt
50
0.024
0.021
0.013
• • •
Amyl alcohol
IS
0.I9I
0.086
0.043
0.014
tt
25
0.236
0.145
0.066
0.018
tt
35
1. 481
0.438
0.104
0.039
tt
SO
4.869
1.893
0.263
0.105
Amyl Acetate
IS
0.II9
0.063
0.039
0.029
tt
25
0.162
0.073
0.045
0.030
u
34.6
0.259
0.105
0.057
0.046
M
SO
1-939
0.605
0.216
o.iis
395 MAQ
HSSIUM HITBATS
KAOHUIUK
nrSATS Mg(NO,)..
Solubility
IN Water.
(F^mk — WiaB. Ahh. p. t.
Gnu.
Mob.
Gms.
Mob.
^^ M«(NO»),
t* periooGms.
Mc(NQ|)i Solid
per 100 IdJob. Phase.
^ M«(NO^
t^. per ICO Gms.
M<(NOO, Solid
per 100 Mob.' Phase.
Solotkn.
HaO.
Solution.
H2O.
-23 35.44
6.6 Mg(N0|)i4»H^
40 45-^7
10.3 Mg(N0ft)|J6^/>
— 20 36.19
7.0
80 53.69
14.6
-18 38.03
7-4
90 57.81
16.7
-18 38.03
7.37 Mg(NO»),iSHK)
89 63.14
20.9 1
- 45 3950
7.92
77 5 65-67
23.2 >•
0 39.96
8.08
67 67.55
25 I 1
+18 42.33
8.9
* Reverse
curve*
(Fahiioo, 1916.)
(Aaseliii, 1873.)
Sp. Gr. of solution saturated at x8^ — x.384.
The eutectic is at —29® and 34.6 gms. Mg(NOs)s per 100 gms. sat. solution.
Fusion-point data for Mk(NOi)i + Zn(NOi)i are given by Vasilev (1909.)
Results for Mg(NOs)i 4- HnOi are given by Demby (1918).
MAQMBSIUM OLEATB (CH,(CH,)i,CH-.;CH.CH,COO),Mg.
One liter HsO dissolves about 0.23 gm. oleate (soap).
100 gms. glycerol (d 1.114) dissolve 0.94 gm. oleate.
MAQMBSIUM OZALATB MgC,04.2H,0.
One liter of water dissolves 0.3 gm. MgCsOi at 18^ (conductivity method).
(Kohlrausch, 1905.)
MAQHESIUMJ OXIDE MgO.
Fusion-point data (quenching method) for MgO + SiQi are ffiven by Bowen
and Anderson, 19 14.
MAQHESIUM PHOSPHATB MgHP04.3H,0.
Solubility of Magnesium Phosphate in Aqueous Solutions of Phosphoric
Acid at 25**. (Camcpon and BcU, 1907.)
The mixtures were constantly agitated for two months and the clear solutions
analyzed for magnesia and phosphoric acid.
^of
Gnu. per Liter.
X.006
X.017
X.042
X.069
1. 109
MgO.
0.207
0.280
O.SS3
1.438
2.23
4.73
IX. 19
X7-33
26.09
X.144 37.40
1-285 75. 5
«^ . SolidPhase.
PA.
0.486 MgHP04.3H^
0.732
X.917
4.8s
• 7. 35
16.84
38.59
61. 2X
93 09
130.7
281.8
Sat. Sol.
X.470
X.595
Gms. per Liter.
MgO.
X09.S
122.6
129.9
140
146.8
PA.
439
498
546.5
584
623.3
Solid PfasM.
MgHPOi-aH^
X.626
X.644
X.654
147-3 625.9
150-3 645.8
155.5 680.7
160 700
87.1 779-6
77.1 809.6
70.6 835.x
«
«
M
M
If
+lifgH«(P0«)tJCH^
MgH«(PO«)t.XH|0
«
n
(Saber, x886.)
MAQNISIUM (Hypo) PH08PHATB MgtPsO<.i2H,0.
One liter of water dissolves 0.066 gm. hypophosphate.
One liter of water dissolves 5 gms. magnesium hydrogen hypophosphate,
MgHsPsOc.4HsO. (Saber.)
MAaNESIUM SALICYLATB Mg(C7HA)2.4HtO.
100 gms. sat. solution in water contain 20.4 gms. salicylate at 15^ (14.3 gms.
Squire and Gaines, 1905)^ and 79.7 gms. at 100 . (Tarugi and Checchi. 1901.)
too gms. 90% alcohol dissolve 0.6 gm. salicylate at 15^-20^ (Squire and Cainci, 1905^
BCAaNSBXlTM SXUCATK 396
MAQMBSIUM 8IUCATE M^SiO..
Fusion-point data for mixtures of MgSiQi + MnSiQi are eiven by Lebedew
(191 1). Results for MgSiOi + NatSiOs are g;iven by Wallace (1909).
MAQNESIUM rLUOSIUCATB MgSiF«.6H,0.
One liter of water dissolves 652 g^ms. of the salt ,at 17.5^. Sp. Gr. of solution
- 1.235- (StoU»,i8770
MAQMBSIUM SUCCINATB CiHAMg.sHA
100 gms. sat. solution in water contain 24.35 8^11^ succinate at 15^ and 66.36
gms. at 100". (Tuiagi and Cheocbi, 1901.)
MAQMBSIUM SULFATB MgS04.7HsO.
Solubility in Water.
(Results by several investigators. 4th Ed. Landolt^and BQmstein, " TabeUeOt
1912.)
ft
f.
-2.9
-3-9
+1.8
10
20
25
30
40
48
SO
55
60
68
80
83
99.4
164
188
Gms. MgSOi
per zoo Gms.
Sat. Sol.
SoUd Phase.
loe
" +MffSO«.iaH«0
MgSO«.z2H,0+B^SO«.7H|0
llgSO«.7H^ (rhombic)
II
II
tt
u
" +KgS0«.6H/)
MgSO«.6HiO
II
it
r.
Gms. MgS04
per 100 Gms.
Solid Phase.
G
Sat. Sol.
Unstable Portions of Curve.
—8.4 23.6 (i) Ice
-5
o 20.6 (3)
3)
" +lifgSO«.H^
KgSO«.H^
o
+10
20
o
10
20
30
70
80
90
100
19 (12) " +MgS04.7H^riKmb.
20.6 (3) MgS04.7H^ rhomb.
/Iheafooal
U M
i<
M
MgSQ|.6%0
M
«
40.6 (10)
29.3 fll^
20.3 (11)
tt
tt
tt
tt
(i) de Coppet, 1872; (3) Cottrell et al, 1901; (3) Loewel, 1855; (4) Basch, 1901; (5) Mulder;
(6) Vander Hcide, 1893; (7) Smith, 1912; (8) Van't Hoff. 1901; (9) Geiger, 1904; (zo) Meyerhoffer,
Z9Z2; (zi) Etard, 1894; (la) Guthrie, Z876. See also Tilden, 1884.
Data for densities of aq. MgSOi 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, Z9Z7.)
Gms. per xoo Gms. Sat. Sol.
llgSOi.
26.76
26.67
26.57
26.36
26.39
18.76
16.36
14.27
K«S04.
O
1.68
2.34
4.02
7.02
8.43
9 63
Solid Phase.
MgS04.7H^
Gms. per xoo Gms. Sat. Sol.
11
If
If
" +MgK«(S04)t.6H«0
MgK«(S04)i.6H^
K
tt
MgS0«.
13.26
12.88
12.68
12.06
10.69
7.8
4
o
K«S04.
10.34
10.51
10.70
10.77
10.84
II. 10
11.03
10.77
SoUd Phase.
MgE«(S04),.6HyO
tt
« +K.SO.
KiSQi
M
W
U
100 gms. 95% formic acid dissolve 0.34 gm. MgSOi at I9^
(Ascfaan, zgzjO
397 MAQMBSIUM SULFATE
S(X.UBIUTY OF MaGNBSIUM SuLFATB IN MbTHYL AND EtHYL AlCOHOLS
(de Bruyn, 1892.)
Solvent. V. Per zoo Gms. Solvent. Solvent. t". Per zoo Gms. Solvent.
Abs. CHiOH 18 1.18 gms. MgS04 93% Methyl Ale. 17 9.7 gms. MgS04.7H^
" 17 41 " MgS04.,HiO 50% " " 3-4 4.1 "
" 3-4 29 " " Abs,CiH|OH 3 1.3 "
SOLUBILITT IN AqUEOUS EtHYL AlCOHOL.
(Scfaiflf. z86i.)
Weight per cent Alcohol lo 20 40
Gms. MgS04.7HjO per 100 gms. solvent 64 . 7 27.1 i . 65
Solubility of Magnesium Sulfate in Saturated Sugar Solution at 31.25^
(KOhler, Z897O
100 gms. saturated aqueous solution contain 46.52 gms sugar + 14 gms.
MgSO*.
100 gms. water dissolve 1 19.6 gms. sugar + 36 gms. MgSOi.
Data for the system magnesium sulfate, phenol, and water are given by Tim-
mermans, 1907.
Fusion-point data for mixtures of MgSOi + K«S04 are given by Ginsberg,
1906; Nacken, 1907a and Grahmann, 1913. Results for MgS04 + Na4S04
are given by Nacken 1907b.
MAQHESIUM POTASSIUM SULFATB MgKt(S04)s.6HA \,
Solubility in Water.
(Tobler, 1855.)
t"= o^ 20^ 30^ 45'* 60^ ys*"
Gms. MgKs(S04)2 per
loogms. H2O 14. 1 25 30.4 40.5 50.2 59.8
100 gms. HtO dissolve 30.52 gms. MgKs(S04)i.6H20 at I5^ (Lothuui, 1909.)
MAQMBSIUM SUUITB MgSO,.6HtO.
10 gms. cold water dissolve 1.25 gms. sulfite; 100 gms. boiling water dissolve
0.83 gm. (Hager. 1875.)
100 gms. HsO dissolve I gm. sulfite at 15^ iSqirat and Caiaes, 1905.)
BCAOMESIUM SULFONATBS.
Solubility in Water at 20*.
(Sandquist, 19x2.)
Magnesium -2-Phenanthrene Monosulfonate 6HiO 0.051
-3- " " 4H,0 0.116
" -i«>. " *« SHjO 0.22
MALAMINXC ACID 398
p UALMMimC ACID CH,(OH)COOH ^CHtCONH,, CHiCOO.NHt.CHCOOH.
Solubility in Water at I8^ (Luu. 1903.)
ri«M«wM.n/i M n» Giii«.pef xoo <a)p in Water
J /3 Malaminic Acid 149 7-52 +9.70
/ " 149 750 -9-33
r " 148 4.02
MALIIC ACID COOHCH::CH.COOH (see also p. 304).
Solubility in Several Alcohols, cnmoieieir, 1894.)
Gms.
Gat.
AloohoL
f.
(CHCOOH)!
per xoo Gms.
Sat. Sol.
Akohol.
f.
(CHCOOH),
per xoo Gms.
Sat. Sol.
Methyl Alcohol
22.5
.41
Propyl Alcohol
0
20
Ethyl Alcohol
0
302
u
22.5
24.3
a
22.5
34.4
Isobutyl Alcohol
0
14.2
((
22.5
17s
Data for the distribution of maleic acid between ether and water at 25^ are
given b^ Chandler, 1908.
Freezing-point data for mixtures of maleic acid and / mandelic acid are given
by Centnerszwer, 1899.
MAUC ACID / COOH.CHsCHOHCOOH.
100 gms. methyl alcohol dissolve 124.8 gms. malic acid at o^ cnmoidew, 1894.)
I9'.
19*.
1 5^ (Welter & Bniiiv, 1894-)
167.7
ethyl " " 914
propvl 54
dichlorethylene " 0.009
trichlorethylene " o.oio
»® <« »»
^ Distribution of Malic Acid between Water and Ether. GPinnow, 1915.)
Results at 15"*. Results at 25.5^
Gm. Moli. Acid per Liter: ^^ _^_ Gm. Moli. Add per Liter. Cj^^iIL
Rfi Layer. Ether Layer. H|0 Layer. Ether Layer.
0.564 0.0091 62 1*179 0.0172 68.4
0.288 0.0045 ^4 0.582 0.0082 71
O.151 0.0024 62.9 0.293 0.0040 73
0.967 0.0157 ^^'^ 0.142 0.0020 71
Freezing-point data for f malic acid + / mandelic add are given by Cent-
nerszwer, 1899.
halonic acid ch,(cooh)i.
m
SoLUBiLtrY IN Water.
(Klobbie. 1897; Miczynski, x886; Hbnry, 1884; Lamooxouz. 1898, 1899.)
Gms. CHt(C(X)H)s per 100. Gms. CHs(C(X)H)t per xoo.
Gms. Solixtion.* cc. Solution (L.). Gms. Solution.* cc. Solution (L.).
o 52 61 50 71 93
10 56.5 67 60 74.5 100
20 60.5 73 70 ... 106
25 62.2 76.3 80 82
30 64 80 100 89
40 68 86.5 132m.pt. 100
* Average curve from results of K., M., and H.
100 gms. 95% formic add dissolve 2242 gms. malonic add at 19.5^. (Aaduui, x9X5.)
399
MALOMIC ACID
SoLUBiLmr OF Malonic Acid m Alcohols.
(Tinoieicir, 1894.)
Gns.
AloohoL
Methyl Alcohol
M
Ethyl Alcdiol
it
it
ii
tt
f.
— 18.S
-15
O
+ 19
+19. 5
-18.S
-IS
o
+19
CH|(COOH),
per 100 Gns.
Sat.SoL
42.7
43-5
47.3
52. S
53-3
30
30.7
35. 3
40.x
Alooooi.
f.
Ethyl Alcohol
Propyl Alcohol
it
«
it
tt
n
tt
tt
tt
Isobutyl Alcohd
tt tt
+19 5
-18.S
-15
o
+19
+19.5
o
19
G188.
pariooGoM.
41.3
19.5
30. a
243
39. S
30.7
17. S
21.2
SOLUBILRT OF MaLONIC AoD IN EtHBR.
(Klobbie, 1897.)
r.
o
10
20
25
Got. CE^OOOH).
per 100 Gns.
6.2$
7.74
9
9.7
Gms. C^C00H)i
t*. per 100 Gns.
Solntion.
30 10.5
80 33
90 39
r.
100
no
Z20
132 m. pt.
Gmt. CH|(C00H)t
per 100 Gns.
Sofaitioa.
46
S6
70
100
100 gms. saturated solution of malonic add in pyridine contain 14.6 gms. at 36^.
(Holty, 190S.)
Solubilitt of Substitutbd Malonic Acids in Water.
(Lamourouz, 1899.)
Gms. per xoo oc. Satnnted Aqueoos Solutioii.
f.
O
15
25
30
Malonfc
Acad.
61. 1
70.2
76.3
92.6
Methyl
Malonic
Add.
44.3
58.5
67.9
91.5
Ethyl
Malonk
AckL
52.8
63.6
71.2
90.8
iiPropyl
Malonic
Add.
45.6
60.1
70
94.4
iiBat]fl
Add.
ZI.6
30- 4
43.8
79.3
bo Amjd
Malouc
AckL
38. 5
51.8
79-3
83.4
Distribution of Malonic Acid bbtwbbn Ether and Water at 25^
(Chandler, 1908.)
Mols. Add per Liter.
H^ Layer.
o. 1478
O.II2X
0.0862
0.0331
MANDIUC ACID
Ether Layer.
0.0135
0.0102
0.0076
0.0027
Coef.
Cone. H^
Cone Ether
10.94
11.07
11.28
12.22
Diit. Coef.
oomcted foe
lonication.
9.86
9-79
9.86
9.82
C«H«.CH(OH)COOH iandd.
S0LU91LITY IN Several Solvents.
Water
(4
Methyl Alcohol
t€ tt
Ethyl Alcohol
u tt
Propyl Alcohol
it tt
9S% Foimic Add
f.
Gms. CHiCHOHCOOH
per loo^Gms. Sat. Sol.
Attthoiity.
20
15.95
(inactive add)
(Scfalonbeig, 190a
20
19.17
(deztioadd)
M
0
51. 1
(inactive add)
(Timoieiew. 18940
16.5
64.9
u
M
0
46.7
M
M
•
16.5
53.6
M
M
0
35
M
M
16.5
43
M
M
19
40
«
CAaditn, 1913^
MANDIUC ACID
400
F&BBziNG-poiNT Data (SolubiHtv, 866 footnote, p. i) Arb Given for thb Fol-
lowing Mixtures op Mandelic Acid and Other Compounds.
d Mandelic Acid + / Mandelic Add
/
(Adruni, 1900.)
** +/ " " (Centnenswer. 1899.)
Methylester + 1 Mandelic Methylester "
Isobutylester + / Mandelic Isobutylester "
Acid + Dimethylpvrone (Kendall 19x4-)
/ Menthylester + a Mandelic / Menthylester (Flndlay and Hkkimm, 1907.
Menthyl MANDBL4T18.
Solubility in Ethyl Alcohol.
(Findlay and Hidunans, 1909.)
Solvent.
f.
Gms. ]
Gms.
aer xoo
Solvent.
P^. Solvent.
f.
Gms. per xoo _ ...
Gms. Solvent. Solid
s , * — =— ^ Phase.
L.
D.
L.
D.
80% Alcohol
35
• • •
1.08
D 80% Alcohol
xo
• • •
0.287 D
«•
35
3.19
• • «
L
10
0.595
L
35
0.80
0.80
R
10
0.184
0.184 it
35
0.544
1.35
D-k-R "
10
0.404
0.291 D-^-R
35
2.83
0.60
L+U
10
0.505
0.088 L-^-R
25
• • •
0-595
D Abs. Alcohol
0
• • «
1.06 D
25
1.64
• • •
L
0
1-93
L
25
0.448
0.448
R
0
0.625
0.625 ^
25
0.321
0.882
D-^-R "
0
0.535
0.915 P+JJ
25
Z.192
0.267
•
((■■"0.8517.
0
X.03
0.54 L+«
P — / menthyl d mandelate, [alj,*^-* = —945* in alcohol.
L — / menthyl / mandelate [ot]j^ » — 140.92® in alcohol.
R ^l menthyl r-mandelate [al|,"-* = —75.03 in alcohol.
nUNQANXSE BORATB MnH4(BQi)s.
Solubility in Water and in Aqueous Salt Solutions.
(Hartley and Ramage — J. Ch. Soc. 63, I37t '93.)
Gfams MnH4(BOs)9 per liter In SolutioDs of:
X4
18
40
60
80
H.O +
trace
NatSO«.
094
...
0.50
• • •
0.08
Na|SO«
Gms.
NasSO«
(o.a Gms. (ao
per liter). per liter).
1.7
0.77
0.69 (52®) 0.65
... 0.36
O.X2
NaCl
(jo Gms.
per liter).
1-31
0.60
0.29
Cadt'
(ao Gms.
per liter).
2.91
2.44
2.25
I -35
Solid
BCANQANESB BROMIDE MnBri.
SoLUBiLrrY IN Water.
(Etaid, X894.)
Gna. MnBik
t*. per xoo Gms.
SolutkiD.
52-3
54-2
56.0
57 -6
595
60. 2
61. z
—20
—10
o
10
20
25
30
MnBrt^H^O
40
SO
60
70
80
90
ZOO
Gms. MnBr«i
per xoo Gms.
Solution.
62.8
64 -5
66.3
68.0
69.2
<59-3
695
SoHd
Phase.
•1
BlnBr.aH«0
401
BCANQANXSI CABBONATI
BCANOANUE CARBONATE MnCOk.
One liter water dissolves 5.659.10-^ mols. MnCQi - 0.065 gn^- at 25*.
(AgeDO and Valla, 19x1.)
BCANQANin CHLOBIDS MnCli.
Solubility in Water.
(Etard; Dawaoo and WUUama — Z. phyaflc. Chem. 31, 63. '99.)
Sp. Gr. of Gtams Maqa per 100 Gfaina
— 20
— ID
O
+ 10
20
30
40
SO
S7-6S
60
70
80
90
100
I30
140
I. 4991
1.5049
I 5343
1-5744
1.6097
1.6108
1-6134
Water.
53-8
$8-7
63 -4
68.1
73-9
77.18
80.71
88.59
98.15
105.4
108.6
no. 6
1X2. 7
114. 1
"S-3
118. 8
"95
Solution.
35 o
37 o
38.8
40.5
425
43-55
44.68
46.96
49-53
51 -33
52.06
52-52
52 98
53-2
53 5
54.3
55 o
Ha]t.Mnai
per xoo Mola. UtP,
Solid
llnCla4H^0«
I*
II 08
M
"•55
12.69
•
14.05
M
15.10
M
15-55
1585
16.14
MnQ>.t^c0
M
M
One liter of water dissolves 87.0 grams MnCl,. One liter of sat. HCl
dissolves 19.0 grams MnCl, at 12^. (Ditto — Compt. rend. 9a, 841. '8x.)
Equilibxuum in the System Manganese Chloiude, Potassium Chloridb
AND Water. (SOsa, 19x3.)
Gma- per xoo Gnu. Gms. per xoo Gma.
Sat. Sol. Solid PluuK. e. Sat. Sol.
f.
6
6
6
28.4
38.4
28.4
28.4
Solid Phase.
MnCli.
40.23
35
•
44
43
38
94
46
28
65
KQ. MnCl^
... MnClf4H«0 52.8 50.14
9.41 " +x.i.a+Ka 58.3 51.72
23.06 KG 62.6 51.86
... MnClf4H^ 62.6 49.95
8.66 " +x.x.a 62.6 44.05
13-79 " +x.2.a+Ka 62.6 36.85
26.91 KQ 62.6
KCl.
6 . 01 MnClt.4H^+MnCl».2H^+i.x.3
MnClt.4H«0+MnCV2H^
MnCli.2H|0
6.67 " +x.x.a
12.49 x.x.3+MnCls.2KCl.aH^
18.77 MnCl|.aKC1.2H|Q+MnCl|.4Ka
31.57 KCl
I.I.2 « MnCU.KCl.2H1O. 1.2.2 = MnCl|2KCl.2HiO
100 cc. anhydrous hydrazine dissolve 13 gms. MnCIi at room temp.
(Webh and Broderson, i9x^).
Fusion-point data for MnCU + SnClt (Sandonnini, 191 1), MnCli + SnCli
(Sandonmni and Scarpa, 191 1), MnCli + ZnClt (Sandonnini, 19 12 and 1914).
BCANQAMBSE CINNAMATB (C<H»CH:CHCOO)iMn.
100 gms. HsO dissolve 0.26 gm. manganese dnnamate at 26^. (De Jong, X909.)
BCANQANXSE FLUOSIUCATB MnSiF6.6HA
100 gms. HiO dissolve 140 gms. salt at 17.5^. Sp. Gr. of solution » 1.448.
(Stolba, X883 )
MANOAME8B H7DB0ZIDE Mn(OH),.
One liter HsO dissolves 2.15.10"* gms. mols. Mn(OH)i at I8^
(Sa(±ur and Fritzmann, 1909.)
One liter HtO dissolves 2.10.10"* gms. mols. Mn(OHi) at 18^. (Tamm. x9xo.)
The determination of S. & F. was made by the neutralization method of Kuster,
that is, by determining the conductivity minimum on adding Ba(OH)s to MnS04
solution and calculating the Mn(OH)i remaining in solution.
nUNOANISE H7DB0ZIDS
408
SOLUBIUTT OF MaNGANBSB HYDROXIDE IN AQUB9U8 SOLUTIONS OP
Organic Salts.
(Tunm, 1910.)
(25 cc. of the neutral salt solution + 25 cc. of aqueous suspension of Mn(OH)s
were shaken different lengths of time. Temp, not stated.)
100 cc. sat. solution in i n sodium tartrate solution contain 0.052 gm. Mn/)4«
100 cc. sat. solution in i n sodium malate solution contain 0.032 gm. MtuPa.
100 cc. sat. solution in i » sodium citrate solution contain 0.095 P^ MniOi*
BCANQANISI ZODOMEBCURATB *3MnIi.5HgIt.2oHsO.
A saturated solution of the salt in water at 17^ has the composition
14 Mnli.HgIt.io.22H|0 and density 2.98. (Duboin, 1906.)
MANOANUl NITRATB Mn(NO,),.
Solubility in Watbr.
(F^mk — WiM. Abh. p. t. Rddunitalt 3$ 4381 '00.)
Gmt. Mob.
MD(NOk}i BCii(NOa)s
per xoo
1. koli.H|0.
7-37 Ma
7 63
8.0
8.4
9.61
10.2
12.0
Sp. Gr. of solution saturated at i8^ - 1.624.
The Eutec is at —36° and 40.5 gms. Mn(NOi)s per 100 gms. Sat. Sol.
nUNQANXSE OZALATB MnC^4.2H,0.
Solubility in Aqubous Solutions at 25*.
(Hauser and Wirth, 1909.)
In Oxalic Acid In Ammonium Oxalate In Sulfuric Acid
Solutions. Solutions. Solutions.
Per 1000 Gnu. Sat. Sol. Per 1000 Gms. Sat. Sol. Per xooo Cms. Sat. Sol.
per xoo
Gms. Sol.
-29
-26
— 21
-16
- s
o
+ 11
43.29
43 IS
44 30
45 5^
48.88
50-49
54.50
Gm.
Mob.
Solid
t«
Mn(NOi)i Mn(NO))t
Solid
Phase.
9
Gm.
too
Sol.
per 100
MolsiltO.
Phase.
0|)s^6H«0.
. 18
57
•33
13 -5
Mn(N0|),.6H|0.
••
25
62
•37
16.7
••
«
27
65
.66
19.2
Mii(N0|)s.3H«0.
M
39
66
•99
20.4
••
«
30
67
■38
20.7
•■
M
34
71
•31
24.9
M
M
35 S
76
.82
33-3
«
G. Mols.
(COOH)^
O
0.0125
0.025
0.050
0.125
0.25
0.49
Gms. G. Mols. Gms.
Mn(C00),.(NH4)t(C00),. Mn(C00)t.
0.312
0.759
0.930
1.080
1.396
1.708
2.081
0.005
0.025
0.050
0.125
0.245
0.245
0.281
0.338
0.479
0.761
1.789
3-970
4 005
4.650
Normality Gms. Solid Phase,
H«SO«. Mn(C00)t.
0.025 1.825 MikC^4.sHdO
0.24 8.850
1 25.95s
2.389 51.080
2 . 987 60 . 109 MiiCi04.sH^+(C00H),
3.952 73.200
4.500 82.401
«
M
«<
II
Results are also given for the solubility of MnCi04.2HtO in aq. solutions of
HtSOi containing also about 0.25 gm. mols. free oxalic acid per liter at 25^
nUNQANSSl OXIDE MnO.
Fusion-point data for mixtures of manganese oxide and silicic acid are given by
Doemickel, 1907.
BCANQANSSl (Hypo) PHOSPHTTS Mn(PHsOs)2H,0.
100 gms. HsO dissolve 15.15 gms. salt at 25°, and 16.6 gms. at b. pt. (U. S. P.).
nUNQANSSE 8XUCATB MnSiOi.
Fusion-point data for mixtures of manganese silicate and titanate are given by
Smolensky, 1911-12.
403
BCANQANSSE SULFATB
BCANQANSSI SULTATK MnS6«.
Solubility in Water.
(CottreD— J. F
byaic
. Ch. 4* 651
, '01; Richards and Fraprie —
Am. Ch. T
. a6L 77, ^1
. The RMdM
linebaiser — Am. Ch. T. I5» '>
u oonfinned by R. and FO
M5» '03i were shown to be inoonect by CottieU. and this coodusioB
GfBms MnSQft per
•
Grams MbSQa per
t*. i<».
Gms.
Solid Phase.
t».
xoo
Gms.
iMMPInw
' Water.
Sdutkn.^
'Water.
Sohilka.'
— lo 47-96
3^ 40
MnSQft.7a^
26
63.94
38-99
UdSQm^O
0 SZ
n
34.73
M
18.5
64.19
39.10
U
5 S6
.24
35-99
M
25
65-32
39 53
M
9 59
33
37- 24
M
30
66.44
39-93
'«
22 61
77
38.19
M
39-9
68.81
40.77
m-
»4-3 63
93
39.00
M
49.9
72.63
43.08
M
S S8
.06
36.69
MnSQ|.5HbO
41.4
60.87
37-84
MnSQ|.%0
9 59
19
37 18
•4
50
58.17
36-76
M
15 61
.08
37.91
M
60
55 -0
35-49
N
^5 64
78
39 31
«
70
52.0
34-23
M
30 67.
76
40.38
M
80
48.0
32 43
M
35-5 71
61
41.74
«
90
42.5
39.83
M
100
34 0
34.34
M
V
SOLUBfLITT OF MaNGANBSB SULFATE, COPPBR SULFATE MiXBD CRYSTALS
IN Water at 18®.
(Stortenbecker, 1900.)
Mols. per too Mob. Mol. per cent
H^. Cuin;
Ctt. Mn. Sdludon. Crystals.
SoHd Phase, CaMnSO«.5H|0. Tridinib
2.282 o 100 100
2.23 0.44
'•54
• ■ •
1-31
3-76
• • •
4.70
[1.06 5.58
90.5
83 -5
74.1
57-7
31 0
29.0
26.1
21.8
21. 2
20.0
15-9
13-9
97-3
95-1
81.3
• • •
70.4
Mols. per 100 Hob.
H,0.
Ctt.
Mol. per eent
____ Cuint
Mn. ' Sblutioa. Crystab.
Solid Phase. CttMnSO«.5HiO. 'McBnic.
[o-73 6.37 10. 27 10. sl
•a. ... S'O 4*9
o*34 7-03 4.66
2.31 2.15
7-375 0.0 0.0
SoUd Phase. CuMnS04. Mnnnrlinic. yH^
20.4 28.2*
15-9
42.6
34-4
22.9]
15.2*
* Indicates meta stabfl pointf .
[1.06 5.58
... ...
to -73 6.37
• . . • . •
... ±8
23-5]
12.45 ^0.8
10.27 16.0]
4.60 $.8*
0.0 0.0
CuMnS04.5HsO - 100-90.8 and 2.1 i-o mol. per cent Cu.
CuMnS04.7HsO « 37.8-4.92 mol. per cent Cu.
Solubility of Manganese Sulfate in Glycol.
joo gms. saturated solution contain 0.5 gm. MnSOi. (do Coniacfc, xgos.)
BCANOANX8E SULFATI
404
Solubility of Manganese Sulfate in Aqueous Solutions of
Ammonium Sulfate at 25^ and 50** and Vice Versa.
(Sfhmnrmakcri, 1909.)
Results at
25^
Results at
50*.
Gms.Der
xooGms.
Cms. per
100 Gma.
SoL
Solul Phase. .
Sat.
Sol.
Solid Phase.
MaS0«.
(NHJ^SO*
MnS04.
(NHJ1SO4.
39.3
0
MnSOvsIM)
36.26
0 1
MnS0«.H/)
38 -49
364
" +!>•
35. 35
2.95
'•+Dt.,
33.44
4.91
Di
30.57
5.14
Dta
22.06
9-65
M
16.86
17.62
H
9.02
20.36
tt
6.92
35.98
U
2.91
37.42
U
6.29
39.71
M
1. 75
42.58
" +(NH4),S04
5.70
43.24
" +(NH4)iS04
1.77
43.24
(NHJtSO*
3.49
44.02
(NHJiSO,
0
43.4
<(
0
45.7
M
D« = MnS04.(NH4)tS04.6H,0.
D«.i =
(MnS04)i(NH4)»S04.
Solubility of Manganese Sulfate in Aqueous Solutions of Sodium
Sulfate at 35** and Vice Versa.
(SchreinemakexB and Provije, 19x3.)
Gms. per too Gms.
. per
Sat.
Sol.
Solid Phase.
Gms. per xoo Gms.
Sat. Sol.
MnSO«.
39-45
33.92
3306
32.92
31.05
27.67
22.14
14.58
NaiSOi.
O
5.23
7.97
7.42
9.20
10.76
14.28
20.01
MnS04.B^
«f
t(
II
+(MiiS04)ff.(Na|S04)M
If
(MnS0«)».(Na|S04)M
If
€t
MnSO«.
Na.S04
13.96
21.91
12.19
22.49
10.45
23.41
7.43
26.58
5.69
29.31
5."
30.52
; Solid Phase.
(MnS0«),.(Na,S04)ia
'* +MnS0«(Na«S04)t
MnSO«.(NaSOJi
i<
u
If
+Na.S04
2.96 31.33
o 33
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; Schrrinrmakeraland Deuae, 1912.)
Results at 25'
Gms. per 100 Gma. Sat. Sol.
CHiOH. MnS0«.
o 39.3
6.81 33.72
liquid layen separate here
53.09 1.23
57.39 0.56
76.70 O
Results at 50^
Solid Phase.
MnS04.5H^
ff
Gms. per loo Gms. Sat. Sol.
ft
fi
MnS04.H^
C|H,0H.
O
6.67
16.02
22.63
36.47
MnS04.
36.26
28.12
18.75
12.54
4.12
SoUd Phase.
'MnS0«.H^
fi
II
Composition of the liquid layers.
Water rich Layer. C|H|0H rich Layer.
%CA0H. %MnS04.
6.81 33.72*
8.48
15.02
31.51
22.61
%CH,OH. %MnS04.
53.09 1.23*
49.76 1.83
32.75 8.01
The following reciprocally saturated meta-
stable solutions were obtained at 50°.
CtHiOH rich Layer.
%CH40H. %MnS04.'
53.64 0.97
Water rich Layer.
% CjH,0H
5.68
7.69
8.70
11.85
%MnS04.
34-95
30.99
29.20
24.84
45.83
41.93
35.15
2.19
3. II
5.95
* These liquids in contact with MnS04.5H^.
^ Similar data are also given for 30^ and for 35^. Both stable and metastable
liquid pairs were obtain^ 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.
r.
CsH(OH rich Layer.
Aqueous rich Layer.
Solid Phase.
fo CH(0H.
% Mn.SO;.
% CH»0H.
% MnSO;.
xo
3706
544
13 78
25 .25
MnS04.5Ut(
IS
44.56
2.79
9.25
29.79
ti
17.
47.11
2.22
8.53
30.88
l€
21
53 SS
1. 10
6.10
35.05
it
2S
53.09
1.23
6.81
33.72
tt
30
45-20
2.49
8.69
30.15
MnS04.HiO
31
43.90
2.74
8.47
30.10
((
3S
41.71
3-44
9.24
28.61
«
37
38.26
4.84
11.03
26.47
((
41
34.01
S.86
11.93
24.97
<(
42
32.37
6.89
13.57
23.09
((
43
31-42
8.51
14.33
22.01
«
Data for the solubility of manganese sulfate and potassium iodate in methyl
alcohol are given by Karpius, 1907.
Solubility of Manganese Sulfate in Aqueous Ethyl and Propyl
Alcohol Solutions at 20®.
(Linebarger, 1B92; Snell, 1898.)
of Alcohol
Gms. HnSO«
per xoo Gms. Aq.
Cone, of Alcohol
in Wt. per cent.
Gms. MnS04
Ethyl Ale
per
xoo Gms. Aq.
. per cent.
' Ethyl Ak.
Propyl Ale.
Propyl Ale.
34
95
6
44
3-3
1.9
36
7.2
4-6
48
2.2
1.4
38
S-8
3S
52
1.4
I.I
40
4-7
2.8
too cc. anhydrous hydrazine dissolve about i gm. MnSOi at room temp.
(Welsh and Broderaon, xgxs.)
Fusion-point data for mixtures of MnSOi + K1SO4, and MnSOi + NaiSOi are
given by Calcagni and Marotta, 19 14.
EtANOANESE SULFIDE MnS.
One liter sat. solution in water contains 71.6.10"^ mols. MnS « 0.00623 gm.
per liter at 18** by conductivity method. (Weigel, 1907; see also Bnmer and Zawadzki, 1909.)
EtANQANESE Potassium VANADATE MnKV»Oi4.8HsO.
100 gms. HsO dissolve 1.7 gms. salt at iS**. (Radan. 1889.)
MANNITOL CHiOH(CHOH)4CH,OH.
Solubility in Water.
(Findlay, 1902.)
A» Gms. CH/)H(CH0H)4CH/)H «• Gms. CH/)H(CH0in«CH^H
*' per ICO Gms. H^. "" per 100 Gms. £^0.
o 759 40 35-4
10 1 1 • 63 (13.94 gms. Campetti, x9oz> 50 . 8 46 . 69
20 17-71 (18.98 gms. Campetti, 1901) 60 60.OI
24.5 20.96 70 74.5
30 25.4 80 91.5
35. 8 29.93 100 133. 1
100 gms. alcohol, Sp. Gr. 0.905, dissolve 1.56 p;ms. mannitolat 14°. (Knisemann, 1876.)
Data for the solubility of mannitol at high pressures are given by Cohen,
Inouye and Euwen, 19 10.
100 gms. sat. sol. in pyridine contain 0.47 gm. mannitol at 26°. (Holty, 1905.)
100 gms. aq. 50% pyridine dissolve 2.^6 gms. mannitol at 20-25**. (I>ehn, 29x7.)
Data for the ternary systems mannitol + succinic acid nitrile + water and
mannitol + triethylamme + water, are given by Timmermans, 1907.
MEBCUBT ACSTATl 406
MEBGUBT ACETATB (ic) Hg(C,H«Oi)i, (otu) Hgk(CHiQi)i.
100 gms. water dissolve 25 gms. mercuric acetate at 10^.
• 100 gms. water dissolve 0.75 gm. mercurous acetate at 13^.
100 oc. anhydrous hydrazine dissolve about 2 gms. mercurous acetate at room
temp, with precipitation of Hg. (Wdih and Bnxfenoo, 19x5.)
MEBCUBT BKNZOATI (ic) (C«H«COO)aig.?H^.
100 gms. HsO dissolve 1.2 gms. mercuric benzoate at 15^ and 2.5 gms. at 100*.
(Tuvgi and Cheocfai, 1901.)
VIECUBT BBOMIDS (ic) HgBr,.
Solubility in Water.
9 Z.06 (Uanigae, tSTeO
25 0.61 (SheniU, X9Q3.)
100 30-25 (Lamigne.)
Mercurous bromide. One liter sat. aq. solution contains 0.000039 8^« HgiBri
at 25*. (SheRitt. I9P3*)
Equilibrium in thb System Mercuric Bromide, Ammonia, Water at 8*^-10*.
(Gaudechoa, 19x0.)
The mixtures were shaken intermittently for 21-48 hrs. Both the dear sat.
Initial Mixture.
Sat. Solution.
Gms. Mols. per
*
Utn,
Gms. Atoms, per ]
[iter.
Solid Pliue.
HgBr,.
KHd.
NHiBr.
' H,.
Br.
N. ^
0.0125
0.0250
0
trace
0.0154
0.0185
(NH&Br)«HgBrt
0.0166
0.0332
0
0.00032
0.0172
0.0202
36% " +64% NHftBrNHiBi
0.025
0.050
0
0.00078
0.0241
0.0251
NHbBr.NHiBr
0.050
O.IOO
0
0.0019
0.0525
0.0514
H
0.0125
0.025
0.0375
0.00178
0.0497
0.0497
M
0.025
0.050
0.075
0.0041
0.103
0.108
M
0.0328
0.0656
0.0984
0.0061
0.133
0.133
93% " +6% NHgBr.3NH.Br
0.0365
0.073
0.1095
0.0060
0.132
0.133
36% " +64% NHgBr.3NH3r
0.050
O.IOO
0.150
0.007
0.170
0.169
NHgiBr.3NH«Br
O.IOO
0.200
0.300
0.0124
0.333
0.338
tt
0.C180
0.036
0.01875
O.OOI
0.0315
0.0318
NHgbBr.NH|Br
0.050
O.IOO
0.006
0.0057
0.X172
O.I178
(1
0.050
O.IOO
0.150
0.0071
0.169
0.168
NHABr.3NH«Br
O.IOO
0.200
0.160
0.0083
0.184
0.187
M
0.125
0.250
0.306
0.0160
0.393
...
M
Solvbjlity' of Mercuric Bromide in Aqueous Salt Solutions at 25*.
(Hers and Paul, 19x3.)
(The mixtures were constantly agitated for eight days.)
InAq.
BaBrt.
In Aq. CaBri.
In Aq.
KBr.
In Aq.
NaBr.
InAq.
SrBri.
Mols. per Liter.
Mols. per Liter.
Mols. per Liter.
Mols. per Liter.
Mob. per Liter.
BaBrs.
HgBrs;
CaBr,. HgBri.'
IKBr.
HgBrt.
NaBr.
HgBr,.
'SrBrs.
HgBr,.
0
0.017
0.072 O.I17
0
0.017
O.118
0.078
0.062
0.104
0.274
0.370
0.645 0.676
0.209
0.098
0.596
0.285
0.328
0.471
0.396
0.540
1.892 1.358
0.770
0.472
1. 142
0.540
0.668
0.90a
0.579
0.759
2.479 2.766
2.380
1.360
2.448
1.276
1. 401
X.770
Z.096
1.478
3-754 3-666
3-470
I 930
5-246
2.306
1.872
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. HgBrt per liter 0.017 0.055 0.088 0.0359 0.611 1.407 2.096 9.5)9
Data for equilibrium in the system HgBri + KOH + U|0 at 25^ are given by
Herz (1910).
4(07 MIBCUBT BBOHIDS
Solubility of Mbrcuric Broicidb in Aqueous Solutions of Mbtyhl
Alcohol, Ethyl Alcohol and of Ethyl Acbtatb at 25*^.
(Hen and Andere, 1907.)
In Aq. Methyl Alcohol. In Aq. Ethyl Alcohol. In Aq. Ethyl Acetate.
wt.%
ch^h
Solvent.
dj^oi
Sat. Sol.
Gms.
HgBrtper
100 oc.
Sat. Sol.
Cil^^
in
Solvent.
dj^d
Sat.SoL
Gms.
HgBrsperi
100 cc.
Sat. Sol.
CHaCQi^
in
Solvent.
d^(d
Sat Sol.
Gnn.
HgBr, per
xoooc
Sat-SoL
X0.6
0.9857
0.72
0
X.0O22
0.60
0
1.0022
0.60
30.77
47 06
64
78.05
0.9588
0.9401
0.9386
0.9744
Z.29
2.52
6.85
14.66
20.18
40.69
70.01
100
0.9717
0.9435
0.9214
0.9873
0.67
1.59
6.58
22.81
4.39
96.76
TOO
I. 0018
I.1159
1.0113
0.574
26.69
14.13
zoo
1.2275
50.25
100 gms. sat. sol. in 95
o®. i6.«w ems. at 25° and
% CHiOH (4, -
22.6.^ frms. at .so®.
> 0.8126)
contain 13.2 gms.
(Reti
HgBn at
lldeCB, XQOO.)
Solubility of Mbrcuric Bromide in Alcohols.
(TSmofeiew, 1894.)
nMel
:hyl Alcohol.
In Ethyl Alcohol.
In Propyl Alcohol.
In Isobi
utyl Alcohol
f.
Gnu.HgBrt
perxooGnu.
f.
Gms. HgBrt
per xooGms.
r.
Gms. HgBrt
per xoo Gms.
r.
Gnu. HgBrt
per xoo Gms.
ch^h.
CAOH.
CH7OH.
C«H/)H.
0
41.15
0
25.2
0
14.6
0
4.61
10
49-5
ID
26.3
10
15.6
10
563
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
713
65
44.5
65
31 -3
65
15.80
6S
90.8
89
66.9
86.5
42.7
97
139 I
Solubility of Mercuric Bromide in Mixtures of Alcohols at 25*.
(Hen and Kuhn, 1908.)
In Mixtures of Methyl In Mixtures of Methyl In Mixtures of Ethvl and
and Ethyl Alcohols. and Propyl Alcohols. Propyl Alcohols.
»«*^ ^-^^ ^a. «i^ ^-^ iS.fk «'«'«• ^•^- 4?iSL
O 0.9873 22.8 O X.227 50.20 O 0.9873 22.80
4-37 0.9932 23.x XI. II 1.X954 47.28 8.1 0.9802 22.25
10.4 1.009 25.4 23.8 I. 1524 41.53 17-85 0.9740 21.06
41.02 X.080 33.3 65.2 1.0257 25.30 56.6 0.9487 17.63
80.69 1. 185 45.7 91.8 0.9437 16.35 88.6 0.9269 14.76
84.77 I.I93 46.8 93.75 0.9368 15.86 91.2 0.9239 14.64
91.25 X.21X 48.6 96.6 0.9275 14.66 95.2 0.9227 14.06
100 X.227 50.2 100 0.92x3 13. 78 100 0.9213 13.78
Solubility of Mercuric Bromide in Organic Solvents.
In Carbon Disulfide. In Other Solvents at i8''-20^.
(Anrtowiki, 1894.) (Sulc., xgoo.)
Gms. ^Brt Gms. HgBrt ^ Gms-K^Brt
t*. per xoo Gms. i*. per xoo Gms. Solvent. Formula. per xoo urns.
Solution. Solution. Solvent^
— 10 0.049 15 0.140 Chloroform CHC1« 0.126
— 5 0.068 20 0.187 Bromofonn CHBra 0.679
o 0.087 25 0.232 Carbon Tetrachloride CCI4 0.003
+ 5 0.105 30 0.274 Ethyl Bromide CjUBr 2.31
10 0.122 Ethylene Dibromide CABis 2 . 34
One liter benzene dissolves 6.99 gms. HgBri at 25^ (Abegg and Shenfll, 19030
MEBCUBT BBOMIDl 408
Solubility of Mercuric Broicidb in an Equimolbcular Mixture of
Ethyl Alcohol and Bbnzbnb. (Dukdaki, 1907.)
t*. o. zo. ao. 30. 40. 5a 60.
Gms. HgBra per 100 Gms. Sat. Sol. 10.7 12 14 16 17.5 19 21
itx) gms. of sat. sol. in acetone at 25° contain 34.76 g^ms. HgBrs. (Rdndets, 190a)
Solubility of Mercuric Bromide in Aniline. (Staronka, z^xo.)
Gms. Gms.
^'dSZ Solid Phase. f. MaL% ^Ig^ sdidPh«e.
C«H»NH«. C«H»NH«.
16.14 HgBrt.2CtH|Nl% HO* 33.3 193. 3 HgBx^aQHiN^
23.83 " 109. 7t 33 S 19s " +HgBr,.CANHi
3S 04 " "S 37-2 229.3 HgBr,.CANHt
53.80 " 120 42.3 283.8
89.64 " 124 50 387.2
116. 9 " 123 SS.4 480.9
• M. pt. t Eutec.
too gms. ethyl acetate dissolve 13.05 gms. HeBrs at i8^ (Naumaim, 19x0.)
100 gms. methyl acetate dissolve 21.93 Sms. HgBri at 18° (da sat. sol. = 1.090).
(Naumann, 1909.)
Solubility of Mercuric Broiodb in Pyridine. (Staronka, 29x0.)
f.
Mol. %
HgBrs.
60
4
70
80
S.8
8.3
90
100
12.2
18.8
TOS
23.2
M
W
Gms.
Gms.
f.
Mol. %
HgBr,.
HgBi«per
zoo Cms.
Solid Phase.
^ Mol. % HgBi^ per
* ' HgBrs. xoo Gms.
Solid Phase.
C»H»N.
CiHjN.
10
S
24
HgBrs.3CAN
I07* 39
291 . 5 HgBrt.aC|H|N+HgBrs
30
8
39 64
•4
no 40.4
309
HgBr^CAN
so
II. 2
S7.49
(1
120 45.5
381-3
u
80
17. S
96.68
tt
1231 so
4SS.8
u
100
22
128. S
M
"5 SI
474-4
3HgBrt.aCAN
XIO
24. s
147.8
f<
130 54 -2
5394
M
ii8t
33-3
227.6
M
I34t 60
683.7
«
IXO
3S.S
250.8
M
133 64
810.4
M
* Eutec. t m. pt.
Solubility of
Mercuric Bromide in Quinolinb.
(Staxooka, 19x0)
•
f.
Mol.%
HgRr,.
Gms. HgBrt per
xoo Gms. C«H7N.
SoUd Phase
88
4.4
12.85 HgBr,.2C9H7N
III
8.9
27.28
((
127
14.3
46.58
u
134
17.6
61.16
it
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 HgBrs + Se are given by Olivan, 1912.
Distribution of Mercuric Bromide Between Water and Benzene
(ThiOPHENE Free) at 25®. (Shenill. 1903.)
B^ Layer.
CfHi Layer.
Dist. Coef.
T
HxO Layer.
C|HeLay«r.
Dist. Coef.
0.017
0.194
0.876
0.00634
0.0715
0.89
O.OII47
0 . 1303
0.88
0.00394
0.0436
0.90
0 00953
0.1074
0.89
0.00320
0.03S3
0.90
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 HgBrs + Hgit in acetone at 25° and
in ethyl alcohol of du = 0.8126 = 95% at o®, 25® and 50® are given by Reinders
(1900). In the case of acetone, the ratio of HgBri in the solution increases with
increase of per cent of HgBri in the solid phase. In the case of the alcohol solu-
tions the ratio in solution does not show such r^ular variations with change of
per cent of MgBri in the solid phase.
409 MBBCUBT CHLOBIDS
MIBCUBT CHLORIDE (ic) HgCU, (ous) HgsCl^
SCX^UBILITY 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.
M Gum. HxC^ per
100 Cms. Sat. SqL
80 23. Z
100 38
120 59
ISO 78 -S
M Gms. HgCli per a*
** zoo Cms. Sat. SoL *'
O 35 25
ID 4.6 30
iS-S S -3 (^'i** 1-047) 40
20 6.1 60
Gins.HgCliper
zoo Cms. Sat. SoL
6.9
7.7
9-3
14
Solubility of Mercurous Chloride in Water.
Gms-HftCli
t*. per 100 Gma.
Sat. Sol.
Authozity.
Gms. HftCli
t*. per xoo Gms.
Sat. Sol.
Atttboiitj.
0.5 0.000140 (Condoctivity. Kohlxausch, Z908.) 24.6 O.OOO28 (Kohlzauach, Z908.)
18 0.000075 (Indirect. Behrend. Z893.) 25 O.OOOO47 (SherriU. Z903.)
18 0.00021 (CondttcUvity, Kohlrausch, Z908.) 43 O.OOO7O (Kohbmuach, Z908O
20 0.000038 (Ley and Heimbadier, Z904.)
Solubility of Mbrcuric Chloride in Aqueous Solutions of
Sodium Chloride.
(Homeyer and Ritsert — Phann. Ztg. 33t 738> '88)
Gms. HgClt per zoo Gms. NaG Solution at:
Per cent Onoentratioa
Kjim.
oi NaQ SolutkiDs.
i^
0.5
zo
z.o
14
S-o
30
zoo
S8
25 0
Z20
26.0 (saturated) 128
6f
13
z8
36
68
Z42
zoo«
44
48
64
no
196
208
Solubility of Mercuric Chloride in Aqueous Solutions op
Hydrochloric Acid at:
(Engd — Ann. cfaim. phys. [6] z7, 36a, '89.)
Mg. Mob. per zoo cc. Sol. Gms. per 100 cc. Sol.
HQ.
4.3
9
17
26
32
34
41
48
70
9
8
9
25
S
I
9
iHga.
9-7
19.8
35 5
55-6
68.9
72.4
85 5
88 6
95 7
HQ.
I
3
6
9
II
12
15
17
35
57
61
49
81
76
48
13
54
84
HgCt.
13 U
18
33
49
58
62
75
87
Z29
04
44
04
80
40
65
70
20
Sp. Gr. of
Solutions.
Z.II7
Z.238
1.427
1.665
Z.81I
1.874
2. 023
2.066
2.198
20-25^ (?).
(Ditte — /Wa.[s] aa, SS^. *8z.)
Parts HQ Parts HgC^t
per 100 per zoo
Parts H|0. Parts Sdutkn
0.0
S-6
zo.z
13-8
21. z
31 o
50.0
68.0
6.8
46.8
73-7
87.8
Z27.4
141-9
148.0
ZS4.0
One liter of o.i » Hg(NOs)i solution dissolves 105 gms. HgCls at 25^
,^^. (MoTM, zgos.)
This result, together with distribution experiments, show that complexes of
HgCIt and Hg(NOi)i are formed.
IBHCUBT CHLORIDS
410
Solubility of Mbbcuric Chloridb in Aqueous Salt Solutions at 2^.
(HetB and Paul. Z9i3-)
•
In Aqueous Ba-
In Aqueous Cal-
In Aqueous Lith-
In Aqueous Mag^-
rium Chloride.
cium Chloride.
ium Chloride.
nesium Chloride.
Mob. per liter.
Mob. per
'CaCI,.
Liter.
Mob. per Liter.
Ua HgOi.
Mob. per liter.
BaO.. HgCl..
MgCl.. HgOf
0 0.265
0,190
0.364
0.414 0.351
0.168 0.374
0.38s 0.697
0.402
0.766
0.835 0.666
0.415 0.719
0.572 I. 167
0.656
1. 108
I. 271 I. 021
0.570 1.131
0.776 1.620
0.964
1. 811
1.738 1.678
0.997 1.864
1.336 2.645
1.429
2.645
2.265 2.214
1.320 2.569
3030 5-343
1-723
3-304
3.091 2.896
1.728 3.206
In Aqueous Potas-
In Aqueous Sodium In Aqueous Strondnm
sium Chloride.
Chloride.
Chloride.
Mob. per liter.
Mob.
per Liter.
Mob. per Liter.
KQ. HgCW.
Naa
HgO,.
SrOf HgC'
0 0.265
0.201
0.372
0.164 0-315
O.I 0.381 (
[SheniU. 1903]
1 0.416
0.508
O.3II 0.563
0.174 0.355
0.671
0.748
0.519 0.829
0.221 0.381
I -153
1. 192
0.724 1.342
0.25 0 . 542 (Shenill. 190S.]
1 I. 941
2.022
1.046 1.776
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.
Gms.perzoc
»Gins.H«0.
lASAVn, Ayw/ , BtM^ ■■WW ACBIUka
SoHdPhM.
wj M.\ntvs mum* j^st^ ««■• lae
Cms. per too Gms. H4O.
KCl.
HgCU.'
KCl.
HgCl,.
0
7.39
HgCU
20.3s
29 HgCli.KCl
1. 12
11.63
t€
26.31
34.83
U
2-39
1572
tt
30 32
39.10
ii
4.05
22.17
*€
34.12
42.82
" +HgClj.2Ka
4.84
25.16
" +2HgCl,.KCl
34.18
39.34
HgCl|.2Ka
5.60
25 13
2 HgCU-KCl
34-34
35.16
(I
6.71
25.66
«
35-54
30 63
€t
7.39
26.41
" +HgCl,.KCl
37.72
24.30
*€
7.46
24.70
HgCl,.KCl
41.33
19-33
" +Ka
8-95
19 -93
•
39-66
15-76
KCl
IS
22.87
it
37.87
10.28
i€
17-57
26.12
(i
35.32
2.1
tt
100 gms. I ft aq. NaCl solution dissolve 25.08 gms. HgCli at 25*.
(Osakm, 1901-08.)
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 HgClt + KOH -f HiO at 25^* are given by
Herz, 19 10.
Similar data for merou-ous chloride + KOH + H^ at 25^ are given by Herz,
1911*
411
MEBCUEIC CHLOBIDS
Solubility of Mixtures op Sodium and Mercuric Chloride in
Water at 25**.
(Foote and Levy — Am. Oh. J. 35* a39» '06.)
Cms. per xoo Gms. Solution. Cms. ptf 100 Gms. Undissolved Residoe.
' iS).
NaQ.
26.5
18.66
18.71
18.64
18.87
14.97
14
12
13
13
03
97
14
IS
HgQa.
none
51 -35
51-32
51 42
51.26
57-74
59 -^^
62.16
62.59
62.50
62. 48
62.55
NaQ.
100
16.38
16.36
16.16
15.96
Two detenninations made at xo.3^ s&ve:
19.46
19.48
46.49
46.50
67.46
22.83
HgCla.
none
16.39
21.98
65.42
71-25
74.18
74.21
74.70
74.76
78.20
88.64
90.83
29.19
68.85
Solid
Phase.
none NaQ
NaQ and
Naa.HBat.aH^
Double Salt
NaaJIgClt.9HsO
Gale. Comp. — i6jox% NaQ
74.14% Hga^.85% HflO
NaajagOfl^HtO
andHgCls
3-35
8.32
Solubility op Mixtures op Potassium and Mercuric Chlorides
IN Water at 25°.
(Foote and Levy.)
Compositian of Solutun.
Grams per xoo Grams
Peroentafle Compod
of UndisBolvea
tion
Solid
Solution.
Residue
PbaM!.
' Ka.
Hga,.
ICCI.
H«Cl,.
HaO.
26.46
none
TOO
none
• • •
KQ
26.24
15-04
■ ■ •
3 63
• • •
26.43
15,02
• • •
26.15
■ • •
KG and
26.33
15.02
• • •
52.01
« • •
aKCliIgCIa.H«0
26.33
14.92
■ • •
61 .04
• • • <
23 -74
18.91
34.61
61.66
3-73'
3.21
aKQJIsCtsJIsO
22.36
21.39
34-77
62.02
L. Gale. Compositioa
34/>S% KCl, 6iA4%Hga»
21-39
23 -88
3480
61.84
3-35.
4.11% HaO
20.32
20.26
27.62
27-38
• • •
• • •
65.24
73 98
• • •
• • •
sKCI JIgCUJIaP and
KaSgOai^
17-85
25-34
21.89
75- 10
3.01^
9.26
18.95
21.02
73-36
5.62
Ka-HgOiJIsO
Calc. Compoeition
ao.sa%Ka. 74^3% HgCI>
4.9S%HaO
7.80
19.56
20.76
73.06
6.18
'6.84
22 -81
20.75
74.54
4.71
6.66
24.32
20.54
73-99
5-47.
6.52
6.64
25-13
25.16
• • •
• • •
76.46
80.60
• • ■
• • •
KQ-^CIsiliO and
KQ^Qs^aHsO
6.27
5-77
25.11
24.73
12.09
11.87
83.20
83.18
4.71
4-95
Ka.aHgas.aH/>
( Calc. Composition
J xi43%Ka 83/>5%HgCli.s.sa%H,0
4.68
24.75
• • «
84.46
• • •
4.66
25-17
• • •
93.68
• • •
Ka.aHgCU.aH«0 and HgClf
4.69
24.82
• • •
98.50
• • •
,
none
6.90
none
100.00
none
HgG.
BBECUBZC CHLORZDS
41a
Solubility op Mixtures of Mercuric and Rubidium Chloridbs in
Water at 25**.
CFoote and Levy, z9o(».)
Compmirinn of SohitibD.
UndiBBolved R^ue.
Gmf-perioo
Gms. Solution.
Solid Phase.
' Rba
HkCU '
Rba
HgCV
H^.
48-57
none
100
none
none Rba
46.76
9.18
88.04
11.24
0.72
47-54
47 55
9-49
9-39
60.33
56.59
37
40
•51
•75
2.16
2.66
RhCl and flRba-HgOfH/)
47-3
9-47
46.73
49
-38
3.88.
47 65
35-16
10 -35
19.58
46.50
45-98
50
50
.92
.80
2 qg aRba.H«CI|.H^ Calc. Com-
*^ po«tioo45.S5% Rba 51.05%
3 -22 J Hga^3^%H*0
34-77
19.94
43-07
52
•44
4.49 aRbaQgC]|.%0 aAd 3Rba
3 . 54 J aHgC^aH*0
34-76
20.10
41.10
55
36
30.27
29.30
20.17
20.55
39-07
39.10
0 £. ^
57
57
34
•47
3-59
3-43
aRbaaHgOfaB^
Calc. CompoBition
38.55% Rba, 57.6a%Hffai.
27 38
20.63
38.67
57'
.40
3-93
3.83% H^
26.83
20.87
38.48
57
36
4.16
3RbCl.aHgCl|.2H^ and
27.09
20.97
31-40
64
%
4.25
RbCLHga,.H^
26.15
20.58
30 -34
65.
4.18
Rba.Hga».H/)
23.81
18.71
30.87
65
10
4.03
Calc. Composition
18.10
14-25
29.87
65
28
4.85
39.49% Rba 66.xz%HgCI|,
10.87
10.42
29-33
66,
IS
4.52
4.40% H/)
10.68
10.56
28.59
67,
99
3 .42 1 Rba.HgCl».B«0 and ^RbQ
I 58[ 4HgCl,.H/)
10.50
10.05
26.23
72.
.20
10.06
9.86
35.28
73'
38
0.84
8.48
8.46
8.71
8.80
25-30
25-44
73
73'
IS
67
1-55
0.89
3Rba.4HgCI|.H^
Calc Composition
34.76% Rba, 74.01% HgCli,
5-68
8.70
25-09
73.
46
I -45
z.a3%H^
S-io
8.33
24.92
73
93
i-iS
3-43
8.25
23.79
75'
72
1.49
1 3Rba.4QgC]|.H^ and RbO
3.38
8
13.68
86.
74
0.58
SHgd,
2.98
7.71
8.40
91.
24
• « •
1.89
7.64
8.38
91.
78
• • •
RbasHgOf
Cslc Composition
1.50
7SS
8.30
9t.
81
• • •
8.ao% Rba 91.8% HgCW
1. 10
7.21
8.07
91.
58
• • •
0.79
0.84
7.16
7.42
6.91
3.27
93'
97-
IS
09
RbasHgClt and HgCW
• • •
none
6.90
none
100
• • •
HbO.
Solubility op Mercuric Chloridb in Acetic Acid.
(Etard. 1894)
f.i
Gms. Ocdi
per looGma.
Solution.
20
2-5
30
35
40
50
60
4-7
6
7.2
f.
Gms. %Clt
per zoo Gms.
Solution.
70
80
8.5
9-7
90
. II
100
12.4
Gms.aKCI|
t*. per xoo Gms.
Solution.
no 13.6
120 16.5
130 20.7
140 25 . 2
160 34.8
413
BSEBCXJBT CHLORIDE
SoLUBiLiTT OP Mbrcukous Chloridb (Calomel) IN Aqueous Solutions op
Sodium Chloride, Barium Chloride, Calcium Chloride and op Hydro-
chloric Acid at 25^
(Richards and Aicfaibdd, 1909.) .
Solid phaae in each caae. Calomel + about 0.1 gm. of mercury.
In Aqueous NaCl.-
1
[n Aqueous BaCl
i>
Sp.Gr.of
Gms.
per liter.
HgO.
Sp. Gr.of
SolntioDS.
Gms. per liter.
SoiutioiM.
' NaQ.
' BaCI,. B
HgO. '
• • •
S'^S
0.0041
1.088
104.15
0.044
1.040
58.50
0.041
1. 134
156.22
0.088
1.078
119
0.129
1. 174
208.30
0.107
1.093
148.25
0.194
1.263
312.54
0.231
1. 142
222.3
0.380
1. 188
292.5
0.643
In Aqueous CaClt.
In Aqueous HCl.
$p.Gr.of
Gms.
Sp. Gr. of
SolotioDS.
Gbm. per Liter.
wftintwOPai
CaCl^
Hga. ^
Ha.j
HbCL'
• • •
39.0
0.022
• • •
31.69
0.034
• • •
55. 5
0.033
• • •
36.46
0.048
1.064
III
0.081
1.642
95-43
0.207
1 . 105
138.75
0.118
1.069
158.4
0.399
1. 151
195.36
0.231
1. 091
209.2
0.548
1.205
257.52
0.322
1. 114
267.3
0.654
1-343
324.67
0.430
1. 119
278.7
0.675
1-315
432.9
0.518
1. 132
317.3
0.670
I -358
499.5
0.510
1. 153
364.6
0.673
100 ems.
bromoform.
CHBra, dissolve o.<
>55 gm. H
IgCl at i8*-20*.
(Sufc., 1900.)
Solubility op Mercuric Chloride in Aqueous Ethyl Alcohol at 25^.
(Abe, 191 2.)
caoh.
HgCW.
Solid Phase.
CiHiOH.
HgCU. • *^""^"^
0
6.80
HgCU
45.84
15.36 HgCli
5.08
6.65
49.86
18.18 "
14.49
6.41
53.61
21.40 "
21
6.5s
57.26
24.51 "
26.25
7.31
cs
60.55
27.67 "
31 53
8.51
63 -95
29.86 "
36.85
10.32
67.39
32.40 **
41.36
12.64
Solubility op Mercuric Chloride
IN Aq. Ethyl Alcohol at 25^
(Hers and Anders, 1907.)
Wt. % CH^H
inSolveiit.
tf*. of Solvent
<f..ofSat. SoL
100 ccTSst. SoL
0
0.9971
1.056s
7.22
20.18
0.9665
I. 02 14
6.76
40.69
0.9302
I. 0180
10.69
70.01
0.8632
I. 0616
23.60
100
0.7856
I. 1067
36.86
MUtCXJBT CHLOBTO 414
SOLURILITT OF MERCURIC ChLORIDB IN AqUBOUS MbTHTL AlCOHCX. AT ^5*.
(Hen and.Anden, i907*)
Wt. % COfilB
insolvent
Js-ofSohreaL
d^oiSut.S6L
Cms. ^CU per
100 cc Sat. S6L
10.60
0.9792
I. 0441
7.90
30 -77
0.9481
I .0420
II. 31
37.21
0.9369
1 .0507
13 -43
47.06
0.9186
1.0809
19.71
64
0.8800
I.20IS
38.44
78.0s
0.8489
1-3314
5717
TOO
0.7879
I. 2160
48.62
100 cc. 90% ethyl alcohol disBolve 27.5 gms. HgClt at I5.5^ du sat. sol. » 1.065.
(Greenish and Snilli, 1903 J
100 ems. 99.2% ethyl alcohol dissolve 33.4 gms. HgCli at 25^ (Onkn, i9Q3-S-)
•^ ahi. " " " 49.5 " ^' " . (de Bruyn, 189a.)
" methyl " " 52.9 " " at 19.5* and 66.0 gms. at 25*.
(de Bniyn, 1892.)
1.2 " " at the crit. temp.
(CentaoBifcr, I9xa)
80LUBILITT OP Mbrcuric Chloride in Methyl, Ethyl Propyl*
n BuTYLp Iso Butyl and Allyl Alcohols.
(Eurd — Ann. chim. phys. [7] a» 56^ '94O
NOTB. — For the solubility in Me, Et, and propyl alcohols at room
temperature, see Rohland — Z. anorg. Ch. 18, 328, '98; at 8.^^, 20® and
38.2 , see Timofejew — Compt. rend. 112, 1224, '91; in Me and Et
alcohols at 25**, see de Bruyn — Z. ph3rsik. Ch. 10, 783, '92. The deter-
minations of these investigators agree well with those of Etard, which
are given below.
Grams HgOa per 100 Grams Saturated Solution in:
t: , K s
CH^H. CtH^H. C^^OH. CHi(CHt)|0H. (CBb)«CHCH^H. CHa£HX%OH
^"*30 ... ^4 *5 ^5*0 ... ••• ...
^20 ... 20.1 15.7 13.5 ... 21.0
— 10 15.2 26.5 16.5 13.7 ... 25.5
O 20.1 29.8 17.4 14.0 $-2 30.0
+ 10 26.3 30.6 18.0 14.3 6.0 37.5
20 34.0 32.0 18.8 14.6 6.8 46.5
25 40.0 32.5 19.5 15.5 7.2
30 44-4 33-7 200 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 33.0 24.9
100 70.1 54.3 43-^ ••• 31-7
120 73.5 6p.s 50.6 ... 39.2
I sO 7^ *5 ... ... ... ... •••
SoLUBiLrrY OF Mercuric CHLORms in Aq. Ethyl Acetate at 25*. ^
(Hers and Anders, 1907.) ^
^^•liS^?* i^ofSol^ .y of Sat. si ^«^^
o 0.9971 I 0565 7.22
4.39* ••• 1.0581 7.38
96.76! ... 1-2371 41. ss
100} 0.884 1.1126 26.42
? A]maitaat.intI»cUi]rla«Ute. f Ethyl acetate alneat sat. with H/>. I(b. pt • 75*77*0 .
415
BSEBGUBT CHLOBIDS
Sqlubility of Mercuric Chloridb in Water-Ether Mixtures at 25^
(Abe, 1912.)
Gms.
pet 100 Gnu. Stt. SoL
Solid Phue.
HgCl,
HgO,.
6.92
S-2
Ether.
87.86
1.2
HiO.
S-22*
93-6
4-3
3.8
S-2
S-4
90s
91.8
il
IS
s-4
931
(€
* (Solvent, ether aat.with H/>.)
Solubility op Mercuric Chloride in Mixtures of Ether and Ethyl
Alcohol at 25^ (Abe, 19x2.)
Gms. per xoo Gma. Sat. Sol. ' Gms. per loo Gms. Sat. Sol.
HgO..
CAOH. '
HgO,.
CiH^H.
32-43
67 -57
36.29
27.16
35-5°
58-59
34.08
22.48
37-39
51.02
28.55
15.20
37-96
44-79
20.67
8.97
38.24
38.69
5-49
0
37-75
32 84
Solubility of Mercuric Chloride in Mixtures of Alcohols at 25*.
(Herz and Kuhn, 1908.)
In Mixtures of Ethvl and In Mixtures of Ethvl and In Mixtures of Methyl and
Methyl Alcohols. Propyl Alcohols. Propyl Alcohols.
%CHiOH j^of
Solvent. Sat SoL
o 1. 107
4.37 I. 130
10.40 I. 157
41.02 1.294
Gms.HgC3s %C|H90H
80.69
84.77
91-25
100
1. 321
1.288
1.254
1.2l6'
per zoocc.
Sat. Sol.
36.86
39-43
42.61
58.37
61.67
57.82
53.85
48.62
m
Solvent.
O
8.1
17.85
56.6
88.6
91.2
95.2
TOO
Sat. SoL
I . 1070
1.0988
1.0857
1.0272
0.9854
0.9824
0.9772
Gms. HgCli % C:^70H
per zoo cc.
Sat. SoL
36.86
36.67
34.06
27.11
21.66
21.60
20.87
20.03
m
Solvent.
O
II. II
23.80
65.20
91.80
93.75
96.6
100
dfyOf
Sat.6ol.
Gms.HgC1f
per zoocc.
Sat. SoL
I. 2160 48.62
1.2278 50.34
I . 2848 57 . 14
I. 1568 42.28
1.0090 25.09
1.0029 23.23
0.9851 21.52
0.9720 20.03
0.9720
Solubility of Mercuric Chloride in Mixtures of Ethyl Alcohol and Ben-
zene AND OF Ethyl Alcohol and Chloroform at Different Temperatures. '
(Dukelski, Z907.)
In a Mixture of In a Mixture of In a Mixture of
two mols. CsHtOH one mol. CsHaOH two mols. CsHK)H
H- one mol. CcHc + one mol. CHiCl. + one mol. CHCU.
Gms. HgCU
t*. per zoo Cms. t*.
Sat. Sol.
In a Mixture of
one mol. CsHiOH
+ one mol. CeH*.
Gi
Sat. SoL
f.
Gms. HgCli
per zoo Gms.
"2.5
o
6
20
20
24
34
54
54
5
65
5
5
4
5
15.20
15-40
16.38
18.40
18.50
19-33
21.34
24.84
24.42
-5.2
o
9.1
20.9
24.4
36.5
53-7
74
19-45
20.13
21.65
23 57
24.19
26.53
31-27
38 -74
-20.5
— 12
o
8
23
38.5
44.2
45-6
Gms. HgCls
per zoo Gms.
Sat. Sol.
82
f.
3
4
4
5
7
8
9
9
43
89
37
12
51
51
98
— 20.5
o
8
23
38.5
44.2
Gms. HsCli
per zoo Gms.
Sat. SoL
6.60
7.69
8.96
10.66
12.50
14.40
Some of the determinations were made b^ 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.
mRCUBT CHLORZDS
416
Solubility of Msrcuric Chloride in Mixtures of Methyl Alcohol and
Chloroform, Methyl Alcohol and Carbon] Tetrachloride, and Methyl
Alcohol and Dichlorethane at Different Temperatures.
(Dukeliki. 1907)
In a Mixture of
In a Mixture of
In a Mixture of
In a Mixture of
one mol. CH<OH
two mols. CHiOH
two mols. CHiOH
two mols. CHtOH
^-onemol.CHCU.
+ one mol. CHCU.
H-one
mol. CCI4.
+ one mol. CsHiCis.
r.
Cms. HkOi
per zooGms.
r.
Gnu. HcOt
per 100 Gins.
r.
Gms.arCls
per 100 Gms.
Gms-HcOi
t*. per zoo Gms.
Sat. Sol.
Sat.SoL
Sat. Sol.
Sat. Sol.
— 12
1-73
— 12
3-33
0
5.20
0 13 -33
0
3SI
0
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
10.15
23
16.56
30.6
19.40
25-3 34.78
24.9
10.71
24.9
18.45
355
20.50
30.2 36.87
30.6
11.40
30.6
19.70
36.1
21.80
37.4 37-95
38. S
12.02
38. s
20.83
48. s
21.90
4S-9 3936
Solubility of Mercuric Chloride in Mixtures of Methyl Alcohol
AND BeNIENE at DIFFERENT TEMPERATURES.
(Timofeiew, 1894.)
In a Mixture of one mol.
In a Mixture of one mol.
CHgOH + one mol. C«H».
CH,OH + two mols. CHi.
f.
Gbm. HfCli per 100
*•
Gms. Hgd per xoo
Gms. Sat. Sol.
m .
Gms. Sat. SoL
0
8
0
4.8
21-25
23 -9
ai-2S
17. 1
30
27.3
30
18
37
28.1
37
18.4
SoLUBiLmr OF Mercuric Chloride in Benzene, in Dichlorethane
AND IN ETHYLACBTATE AT DIFFERENT TEMPERATURES.
(DukeUi. 1907.)
In CsH«.
In C,H4C1,.
In CHiCOOCH,.
r.
Gms. HgCU per
i*
Gms. HgClt
per
*•
Gms. HgCli per
zoo Gms. Sat.
Sol.
« .
xoo Gms. Sat.
Sol.
m •
xoo Gms. Sat. Sol.
6.5
0.26
0
1-33
0
22.9
18
0-53
".5
^'S5
6-5
22.7
34.1
0.64
2S-3
1-73
26.1
22.8
54. 1
1.02
33
2.05
38.5
. 23.5
69
1-39
459
2.42
a
4S-3
26.4
Solubility of Mercuric Chloride in Mixtures of Benzene and' Ethyl-
acetate, Chloroform and Ethyl Acetate and of Carbon Tetrachloride
and Ethyl Acetate.
(Dukelski, X907.)
In a Mixture of one mol.
CeH» -f one mol.
CHiCOOCtHs.
In a Mixture of one mol.
CHCU "f one mol.
CHjCOOCiH,.
In a Mixture of one mol.
CCI4 H- two mols.
CHiCOOCHi.
f.
Gms. HgCli par
A* Gms.
HgOiper
*•
Gms. Hgdiper
xoo Gms. Sat. Sol.
* ' xoo Gms. Sat. SoL
• .
zoo Gms. Sat. SoL
0
9.62
0
3-34
0
9.24
6.5
9.62
26.1
4.07
10.3
9 05
257
9.78
36.1
4.78
25.7
932
27.6
9.98
46
S.38
87.6
.950
355
10.81
48.5
S.io
38. s
989
45 -3
13.69
453
11.70
417
MEBGUEIC CHLOBIDE
Solubility op Mercuric Chloride in Ethyl Acetatb and in
Acetone.
(Etaid. 1894; voD LMspynaki, 1894; Knig and McElzoy, 1892; Linebarger, 1894; Aten, X905-0&)
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.
Gfmms HgOt per xoo Grams Solution.
Gms. RgOs per xoo Cms. Solution.
» . t
Aten.
lioebarger.
Etaid.
—10
* . •
«3'o
• • ■
40
0
22.0
23.2
32.0
40
+10
22.2
n<i
32. s
40
20
22.5
23 -4
327
40
2S
22.7
23 5
33 0
40
30
23.0
33-2
40
40
23-5
33-5
40
50
24.0
33 S
41
60
24.7
• • •
42.5
80
26.0
• • •
4S-2
100
* . •
• • •
48.0
120
...
• ■ •
50.8
150
• . •
■ • •
^S'^
(•) SoUd phaK Hgas(CHa)aCO.
KandMcE. Laszqmski. Aten.
Etard.
44.0* S7«o
49.7 430* 61.7
52.0 Si-o -S8-9t 61.7
37-4
54
S8st
61.7
55-2
SS.a.t
61.7
...
• • •
61.7
• • •
61.7
• • •
61.7
• • •
61.7
-
• • •
• • •
61.7
...
• • •
• • •
• • ■
• 0 •
(t) Solid FhaM HgOi.
100 gms. absolute acetone dissolve 143 gms. HgClt at 18**. (Naumaim, 1904.)
too gms. ethyl acetate ((fy = 0.8995) dissolve 48.8 gms. HgClt at 18^.
(Naumann, X9xo.)
too gms. methyl acetate (d!y = 0.935) dissolve 42.6 gms. HgCls at I8^
(Naumann, X909O
Solubility of Mercuric Chloride in Several Solvents.
(Arctowiki, 1894; von LasKymki, X894; Sulc, X900.)
In Carbon Bisul-
phide (A.).
In Benzene
(von L.).
In Several
at 18-30'
Solvents
' (S.).
f.
Gnu. HgQi
per XOO Gms.
Solution.
f .
Gms. HgOs .
per 100 Gms.
Solution.
Solvant.
Gnu. HgOs
per xoo Gnu.
SdTent.
— 10
0
10
IS
20
O.OIO
0.018
0.026
0.032
0.042
IS
41
84
OS37
o.6i6
0.843
1.769
CHBr,
CHCl,
CCI4
C,H,Br
CH,Br,
0.486
0.106
O.ooa
2.010
X.S30
25
30
0053
0.063
MEBCUBY CHLOBIDE
418
Solubility of Mercuric Chloride in Mixtures of Acetone and Benzene,
Ether and Chloroform and of Ethyl Acetate and Benzene at 25°.
(Marden and Dover, 1917.)
In Mixtures of
CH,COCH, + C«H,.
Gms. CHaCOCHa Gms. HgCU
per 100 Gms. per zoo Cms.
Muctiue.
ICO
90
80
70
60
SO
40
30
20
10
o
Mixed Solvent.
140
117
77
60
45
314
20
10.7
3-9
0.66
In Mijctures of
(C,H»),0 + CHCU.
In Mixtures of
CH.COOCH1 + C«H«.
Gms. CHCU
per xoo Gms.
Mixture.
O
10
20
30
40
SO
60
70
80
90
100
Gms. HirCli Gms. CHgCOOCiHt Gms-HfOt
per xoo Gms. "
Mixed Solvent.
per zoo Gms.
Mixture.
6.9s
4.73
3.70
2.80
2.10
1.48
0.9s
0.657
0.328
0.128
100
90
80
70
60
SO
40
30
20
10
o
per z<
Mked
zoo Gms.
Solvent.
49-3
26
22.1
18. 1
14.2
II
8
5-4
31
1.6
0.66
• Solubility of Mercuric Chloride in Benzene.
(Average curve from results of Linebarger, Z895; Sherrill, Z903; and Marden and Dover, Z9Z7.)
V.
Gms. HgClf per
zoo Gms. C|H«.
f.
Gms. HgCL per
zoo Gms. CA.
0
0.20
25
0.64
10
0.39
30
0.71
20
0.56
40
0.84
Solubility of Mercuric Chloride in Absolute Ethyl Ether.
(Etard, Z894; Lasscynski, Z894; K5Uer, z879-)
i*.
Gms. HgOtper
xoo Gms. Solution.
f.
Gnu. HgCUper
100 Gms. Sonitioo.
f.
Gms. HgClt per
zoo Gms. Solution.
— 20
6
60
6
90
75
0
6
70
6.4
100
8
20
6
80
7
1 10
8-5
Solubility of Mercuric Chloride in Chlorinated Hydrocarbons at 25^
(Hoffmann, Kirmreuther and Thai, 1910.)
Solvent.
Formula.
Ethylene Chloride CHjCLCHia
Tetrachlorethane CtlhCU
Chlorofonn CHCU
Pentachlorethane CsHCk
Gms.
HgCljper
zoo Gms.
Solvent.
1.229
0.090
O.IOI
0.0193
Solvent.
Dichlorethylene
Trichlorethylene
Tetrachlorethylene
Carbontetrachloride CCU
Gms.
Solvent.
CHCl.CHCl 0.114
CHCLCOt 0.0274
CCls.CCli 0.0072
trace
(Aschan, Z9Z3.)
100 gms. 95% formic add dissolve 2.1 gm. HgCU at 19^.
100 gms. 95% formic add dissolve 0.02 gm. HgsCls at 16.5®.
100 cc. anhydrous hydrazine dissolve i gm. HgCk with decomp. at room temp.
(Welsh and BroderM», 19Z5.)
100 cc. anhydrous hydrazine dissolve i gm. HgsCls with decomp. at room temp.
(Welsh and Brodcrson, Z9Z5.)
100 gms. glycerol dissolve 80 gms. HgCls at 25^. (Moles and Marquina, Z9Z4.)
100 gms. glycerol dissolve 8 gms. HgClt ? HgsCls at 15-16^. (Ossendowski. Z907.)
100 gms. anhydrous lanolin (m. pt. about 46 ) dissolve 1.55 gms. HgCls at 45^
(Klose, Z907.)
419 MEBCUBT CHLORINE
SOLUBmiTY OF MbRCUUC CHLORIDE IN PYRIDINB.
(McBride, 1910.)
The determinations at the lower temperatures were made by stirring an excess
of HgCli with pyridine and analyzing the sat. solution. Those at the higher tem-
peratures were made by the synthetic method.
Gnu.
Cms.
^ HgCUper
* * xoo Gma.
Solid Phaw.
f.
HgCUper
xoo Gma.
Solid Phaae.
Sat. Sol.
Sat. Sol.
—32.6 2.76
Hga,.i
iQH^
94.7
60.72
HgCI«.9CAN+3Hgai.3CAN
— 21.7s 7-86
M
74.7
48.38
HgClt.C|H»N(iinstable)
0.02 13.14
M
83.5
50.53
ff
(stable)
12.58 17.34
U
90.4
53.41
ff
If
Z8.78 19. 78
M
97
56.45
If
ff
27.23 22,65
M
100.5
57.84
ff
ff
31.05 24.46
M
104.2
60.72
<i
ff
40.90 29.29
«/
X07
63.06
II
(unstabk)
50.10 34.94
M
106.2
• • «
M
+3HgCl^aQH.N
60.03 4036
If
95-2
60.77
3HgCl|.3CAN (uiMUbk)
70.15 46.44
«
106.4
61.93
(fUble)
76 ...
" +HgCl^CiHiN
Z09.8
62.58
ff If
80.02 51 53
HgCl,
1.3CAN (unsUbfe)
114
63.18
<l M
89 56.45
ft ff
Z24.2
65
a a
94.1 60.09
f< if
145 -5
69.66
M It
Data for this system are also given by Staronka (1910).
Data for the solubility of HgCls.2C»H»N and of Hg(N0i)s.2C»H»N.2H^ in
aqueous solution of pyridine at i8°.i are given by StrOmholm (1908).
Data for the solubility of diamine mercuric chloride, (NH«)tHgCli — NHtHgCl^
in aqueous solutions of ammonia at 17.5° are given by StrOmholm (1908).
Solubility of Mercuric Chloride and op Double Mercuric and
Tetra Methyl Amine Chloride (CH,)4NC1.6HgCla in Aq. Ether
AT 1 7 • (StrOmholin — J. pr. Ch. [a] 66^ 443, 'oa; Z. physik. Cbem. 44, 64, '03.)
Molecular Coooentratian per Liter. Grama per Liter of Solution.
-•*■ ■ ' -% ■* ■ ^
H,0. HgQaC*). Hga2(t). HjO. HgQaC*). Hga,(t).
CO 0.1515 0.0342 o 41.16 9.26
0.0656 0.1795 00428 I. 18 48.64 11.60
O.I3II 0.2069 0.0516 2.36 56.08 14.00
0.1956 0.2339 00603 3.52 63.38 16.34
O.261I " 0.2489 00690 4.70 70.16 18.70
0.3267 0.2849 00779 S-^ 77.20 21.10
0.3922 0.3100 0.0866 7.06 84.02 23.48
(*) Results in this cdumn are for solutions in contact with the Solid Phase HgGs. (t) Results In
this column are for solutions in contact with the SoUd Phaae <CHs)«Naj6HgCls.
Solubility op Mercuric Chloride and op Double Mercuric and
Tetra Methyl Amine Chloride in Alcohol-Ether Solutions
at 17°. (StrOmholm.)
GnmsCsH^H per liter. Grams HgQsC*) per Liter. Grams HKls(t) per Liter.
0.0 41.16 9.26
4.58 5000 11.87
9.16 S^'7^ 14 38
13.74 66.96 16.90
BSEBCUBT CHLOBIDS 430
Solubility of Double Mercuric Chlorides in Aqueous and Pure
Ether at 16.6".
(Strflmhalm, 1902, 1903.)
MoL CoDC. of HgCli per Liter of: Gms. HgCU per Liter of:
Pure Aq. Aq. Aq. Pure Aq. Aq. Aq. Solid Phaie.
Ether. Ether Ether Ether Ether. Ether Ether Ether
(i). (2). (3). (4). (S). (6).
0.1515 0.2387 0.2647 0.3196 41.04 64.69 71.71 86.58 Hgdi
0.0673 0.1157 0.1293 0.1617 18.23 31.41 35.05 43.79 (CH..CH,CA),Sa.6H«CI«
0.0404 0.0720 0.0835 01034 10.95 19-51 22.61 28.01 (CH,.CACH,CiHJ»SCL6H«C^
0.0342 ... 0.0706 ... 9.26 ... 19.10 ... (CH^4Na.6HgCl|
0.0264 ... 0.0568 ... 7.14 ... 15.39 ••• (C,H,)^a.6HgCl,
0.0209 0.0400 0.0460 0.0594 5.66 10.83 12.48 16.10 (CHa C»Hi)tSa.6H«Cl|
0.0063 ... 0.6144 ... 1.70 ... 3.90 ... (CH,),.HiNCLaHgai
(x) oontaining o.axos5 mol. H«0 per liter, (a) 0.2756 mot. H|0 per liter. Cs) 0421 molH/) per liter.
(4) contaioing 3.79 gms. HiO per liter. (5) 497 gms. HiO per liter. (6) 7.59 gms. HiO p«Titer.
Solubility of
Mixtures of Mercuric
•
AND P(
OTAssiuif Chlorides at 25* in:
Absolute Alcohol. (FooCe, 19x0.)
Acetone. (Foote, 19x0.)
Gms. per xoo Gms.
Gms. per xoo Gms.
Sat. Solution.
Solid Phase.
Sat.S<
KCl.
>lution. Solid Phase.
RQ. HgCl|.
HgCl,.
0.21 33.69
Hgai+sKa.6HgCl«aC,H«0H
1.27
61.87 HgCl»+Ka.5HgClt.(CH«>iC0
0.28 33.80
«• «
1-39
60.68 Ka.5HgCl..(CHi)tC0
0.22 24.84
sKa.6HgCl«.2C|H^H
2.58
55.85
0.28 6.21
(f
2.78
54.41 " +5-6. J .
0.25 1.65
sKa.6Hgag.2CAOH+Ka
2.93
48.13 S^a
0.17 1.57
» «
2.52
18.04 «
.0.38 1.03
w "
3-34
13 . 26 "
2.92
II " +Ka
5.6JI = 5KC1.6HgCliJi(CH,),CO.
100 gms. of s^t. abs. alcohol solution of HgCU + NaCl contain 46.85 gms.
HgCls and 3.01 gms. NaCl at 25**. (Foote» 19x00
Solubility op Mercuric Chloride and Sodium Chloride in Ethyl
Acetate at 40®.
(LinebazKer — Am. Ch. J. 16^ 2x4, '94.)
Mols. per
xoo Mob.
Gms.
per 100 Gms.
Gms. per xoo Gms.
Acetate.
Acetate.
Solution.
Solid
KaQ.
HgOs.
Naa.
HgCl,:
NaQ.
HgCl,.
A UHBB.
0.8
13.9
<»S3
39-7
0-53
28.4
HgOt
2-3
12.4
1-53
38 15
i-Si
27.61
M
4-3
16.4
2.85
50-44
2.78
33 54
M
9.1
22.85
6.0s
86.14
5.60
46.28
•■
18.5
34-9
12.39
107.4
10.95
51-76
M
20.0
40.0
13.29
123.0
"•73
55-18
Hgda + Naa
The double salt <HgCla)s.NaCl is formed under proper conditions.
Distribution of Mercuric Chloride Between Water and Benzene.
(Linhart, 19x5.)
Results at 25^ Results at 40"*.
Mols. HgCly per Liter: Cone, in H^ Mols. HgOj per Liter; Cone in H^
CA Layer. HsO Layer. Cone, in CA C^ Layer. H|0 Layer. Cone, in CA
0.02100 0.2866 13.65 0.02647 0.34600 13.07
0.01224 0.15777 12.91 0.015296 0.18470 12.08
0.005244 0.064756 13.35 0.011774 0.138228 XI. 74
0.000618 0.007382 11*95 0.008041 0.091959 XX. 44
0.000310 0.003696 11.90 0.004140 0.04586 XX. 08
0.000155 0.001845 11.90 0.000847 0.009x53 10. 8z
421
BSEBCUBT GHLOBIDS
Distribution of Mercuric Chloridb bbtwbbn Water and Ether.
(Hantach and Sebalt, 1899.)
jo cc. ether + 50 cc. sat. aqueous H^Clt solution were shaken toeether at
different temperatures and after equilibrium was established the HgCU in each
layer determmed.
Mols. HgCli per Liter:
O
10
17. S
25
H«0 Layer (cO-
0.0056
0.0066
(CH,)/) Layer (c«).
0.01407 0.391
O.OI415 0.467
0.0090 0.02150 0.419
0.0095 0.02076 0.429
Determinations by Skinner (1892) at room temp, using concentrations of
HgCls 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 HCl and Ether
AT I8^ (MyUus, 19".)
When I gm, of Hg as HgCU is dissolved in 100 cc. of HsO or aqueous HCl 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. HCl o (=H20) i lo 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.)
Gnu. HisCli per zoo cc Gms. BgOt per too cc.
Layer.
Layer.
Layer.
Layer.
0.443
0.0270
1. 816
0.130
0.732
0.0488
3.766
0.292
0.780
0.0542
3 -754
0.298
1.19a
0.0812
6.688*
0.528*
*.Tliis solution Batuiatod.
Results at Dif. Temperatures.
■
Results at 25"*.
(Hantzsch and Vagt, 190X.)
(Morse, iQoa; Drucker, 1913
Hantzsch and Vagt, 1901.)
1;
Mols. HgCls per Liter:
Mols. HgCli per Liter:
fi.
H^ Layer (ci)-
C|H,CH, Layer (cj).
HtO Layer (ci).
C,HtCH«Uyer(c^.
c»
0 0.0578
0.0047
12.35
O.184IO
0.01590
II. 6
10 O.OS7S
0.0050
11.60
0.09193
0.00807
11.4
20 0.0576
0.0050
11.40
0.04593
0.00410
II. I
30 0.0574
0.0051
11.20
0.02289
0.002II
10.8
SO 00573
0.0052
11.25
O.OII42
0.00108
10.5
0.00573
0.00057
10
Data for the effect of Hg(NOs)s upon the distribution are given by Morae
(1902). Results for the effect of ZnCls 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.)
4- Selenium (Olivari, 1909.)
-f Sulfur
-j- Nitrobenzene (Mascarelll, 1906.)
-torn and p Nitrotoluene (Mascarelli, 1906, 1907, 1909.)
• -j- Urethan ( " 1908, 1909.)
-j- *' + Of Nitronaphthalene ( " 1906, 1907.)
4- " -bp Nitrotoluene ( " 1908.)
4- a Nitronaphthalene ( " 1906, 1907.)
4" P Nitranisole ( •« 1906.)
BSEBGUBT CINNAMATE
422
MEBCUBT CnVNAMATE (ic) (C«H»CH.CHCXX»sHg.?HA
100 gms. H«0 dissolve about 0.03 gm. mercuric cinnamate at 25^ (De Jaag, 1906.)
100 gms. HsO dissolve about o. 53 gm. H g cinnamate at i oo*^. (Taragi ft Cheocfai, 1901.)
MEBCUEIC CTANIDS Hg(CN),.
Solubility in Water.
Gms. Hg(CN)t per loo:
.Gms. H4O. Gc. Sat. Sol.
— o.45£utec. about 11
135 9.3
1$ 12. S
20
25
25 11.27
loi.i 53.85
Authority.
(Guthrie, 1878-)
(TInioCeiew, 1894.)
(lianh and Strathen, 1905^
(EodowbIow, 1898, 1899.)
(SherriU, 1903.)
10. 95 ('^""1^X3) (Hen and Anden, 1907.)
9.3
II. 12
((Griffiths.)
One liter 5.2% aqueous NH| solution dissolves 204.3 S^nis. Hg(CN)s at about 20^
(KoDowalow, 1898.)
SOLUBILITT OF MbRCURIC CyANIDE 'iN AqUEOUS POTASSIUM CYANIDB SOLU-
TIONS AT 25". (Sherrill, 1903.)
Mob per Liter. (jms. per Liter.
KCN. ^ Hg(CN)«. IlCN! " Hg(CN);.
0.0493 04855 3-21 122.6
0.0985 0.5350 6.41 135.2
0.1970 0.6270 12.83 158.4
The rc»:ularity of the increase in solubility proves that the complex Hg(CN)s-
KCN b K>rmed at the given concentrations.
Data are also siven for the distribution of Hg(CN)s between aqueous solu-
tions of KCN and ether at 25**.
Solubility OF Mercuric Cyanide in Aqueous Solutions of Methyl Alcohol,
Ethyl Alcohol and of Ethyl Acetate at 25**. (Hexz and Anders, 1907.)
In Aq. Methyl Alcohol.
Gma.
<M o« H«(CN),
Sat. Sol. P«»«>«-
Sat. Sol.
1.0640 11.02
1.0484 12.46
1.0426 16.37
I. 0441 20.48
1.0484 24.58
1.0762 34.29
Wt. %.
CHdOHin
SoFvent.
10.6
30.77
47.06
64
78 05
100
In Aq. Ethyl Alcohol.
Sat. Sol.
Wt. %
(^HtOHin
Solvent.
In Aq. Ethyl Acetate.
Gms.
.. of
O
20.18
40.69
70.01
100
I. 0813 10.95
1.0339 8.76
1.0006
0.9419
0.8552
9.02
9.57
8.19
in Solvent.
O
4.39
96.76
100
Sat. Sol.
1. 0810
1.0798
I . 9374
0.9097
Hg(CN)t
per zoo oc.
Sat. Sol.
10.95
XO.83
2.66
1.80
Solubility of Mercuric Cyanide in Ethyl Alcohol, Methyl Alcohcx.
AND IN Mixtures of the Two.
In Ethyl Alcohol. In Methyl Alcohol.
^;?^¥«fn^;S^y'" (Dukebki. .90,.)
Gms. Hg(CN)i
t*. per zoo Gms.
Sat. Sol.
8.3
8.8
o
10
20
25
30
40
* d.
Gms. Hg(CN)i
t". per zoo Gms.
Sat. Sol.
26.10
d[y of
Sat. Sol.
9.25
9. S3*
9.8
10.3
'O.8552
O
14-17
234
27.4
31.7
38.1
44.5
29.17
32.01
31 -77
32.53
33- 29
34-05
100 gms. of a sat. solution of Hg(CN)s in a mixture of equimolecular amounts
of CHiOH and CeHs contain 10.2 gms. Hg(CN)t at lo^ 13 gms. at 30^ and 15
In CHjOH+CiHiOH at 25'.
(Hers and Kuhn, 1908.)
%CH^H
in
Mixture.
4.37 0.8618
0.8707
0.9267
1.024
1.034
1.052
1.076
10.4
41.02
80.69
84-77
91.25
100
Gms. Hg(CN)i
per xoooc
Sat. SoL
9.02
10.10
16.70
28.20
29.60
30
34.30
gms. at 50 .
(Dukelski, 1907^
4^3
mRGUBT CTANIDB
SOLUBILITT OF MERCURIC CYANmE IN MIXTURES OF PROPYL AND MbTHYL
Alcohols and Propyl and Ethyl Alcohols at 25^. (Hen and Kuhn, 190S.)
In CsH,OH+CH^H.
In QHTOH+CtHtOH.
A
%C.H,0H
in Mixed
Solvent.
O
II. II
23.80
65.20
91.80
93.75
96.60
100
4m ^
Solvent.
0.7878
0.7894
0.7907
0.7954
0.7992
0.7995
0.7999
0.8004
Sat. Sol.
1.0760
1.0327
0.9891
0.8800
0.8376
0.8335
0.8322
0.8283
Gms.
Hg(CN),
per xoocc
Sat. Sol.
34.3
29.52
24.48
10.48
504
4.23
3.98
3-44
%C|H,OH
in Mixed
Solvent.
O
8.1
17.85
56.6
88.6
91.2
95.2
100
Jy of
Solvent.
0.7867
0.7886
0.7902
0.7926
0.7973
0.7979
0.7986
0.8004
</y of
Sat. Sol.
0.8552
0.8549
0.8527
0.8386
O.83II
0.8306
0.8293
0.8283
Gms.
Hg(CN),
per 100 cc.
Sat. Sol.
, 8.91
7.90
7.30
5-21
3-87
3.84
3.64
3-44
100 gms. acetonitrile (b. pt. 81.6®) dissolve 9.58 gms. Hg(CN)s at 18
(Timofeiew, 1894.)
100 gms. propyl alcohol dissolve 3.79 gms. Hg(CN)i at 13.5**.
' ' ■ - "Tg(CN]
(Naumann and Schier, 19x4.)
't'l
49 58.5 65
77
83.5 84 88.5
100 gms. benzonitrile (b. pt. 190-1*^) dissolve 1.093 8^s. Hg(CN)s at 18**.
(Naumann, 19X4O
Solubility of Mercuric Cyanide in Anh^ine. (Stuonka, 19x0.)
t° of Solidification 41°
Mol. % Hg(CN)a in sat.
Solution 3.7 5.7 7.7 9 14.2 18.2 19.7 23.4
The solid phases are the unstable Hg(CN)s.4CcHtNHs and the stable Hg(CN)i.
2C«HsNHs (m. pt. about 90^).
One liter sat. solution in ethyl ether contains 2.53 gms. Hg(CN)s at 25*.
(Abegg and Sherrill, 1903.)
100 gms. glycerol dissolve 27 gms. Hg(CN)j at 15.5**.
SOLXTBILITIBS OF MbRCURIC CyANIDB DoUBLB SaLTS IN WaTBR AND
IN Alcohol.
1\miM* <U1t ±^
Gms. per
100 Grams.
OI^Mirwr
UfMUMB OKttt w .
Warier.
Alcnhcd. ^
v/DBerres.
Hg(CN),.2KCN cold
22.7
• . •
Hg(CN),.2TlCN i«
12.6
...
(FromuUer — Ber. tz, os» '98.)
Hg(CN),.aTlCN lo^
9-7
...
M tt
aHg(CN),.CaBr,.5H,0 cold
100. 0
50.0
(Cttster.)
2Hg(CN)a.CaBr,.5H,0 boiling
400.0
100. 0
u
Hg(CN),.KCl.H,0 18°
14.81
• • •
(BrettO
Hg(CN),.KBr.2H,0 18°
7-49
• • •
*m
Hg(CN),.KBr.2H,0 boiling
100.0+
• • •
*m
Hg(CN),.BaI,.4H,0 cold
6.42
4.42
(Custer.)
Hg(CN),.BaI,.4H,0 boiling
250.0
62.5 (90% Ale)
Hg(CN),.KI cold
6.2
1.04 (34° B Ale.) (CiJnot^
Hg(CN),.NaI.2H,0 i8°
22.2
15.4 (90% Ale.) (Cm»o
Hg(CN),.SrI^6H,6 'ig^
14.3
aS-o (90% Ale)
Solubility of Mecuric Cyanide in OROAiac Solvents at i8'-2o*.
(Sulc.
1900/)
soncDu
PcfTIWlMi
G.QK(CN)iper
100 Gms.,Solfat.
Bromoform
CUBr.
o.oos
Carbon Tetra Chloride
CCI4
o.ooi
Ethyl Bromide
QHjBr
0.013
Ethylene Di Bromide
CABr,
o.ooi
Data for the ternary system, mercuric cyanide, phenola water are given by
Tumnermaosi 1907.
MBBCUBT CTANIDS
424
Solubility of Mercuric Cyanide in Pyridine. (Staioaka, 19x0.)
Mob.
Hg(CN},
t*. per xoo Mob. Solid Phue.
Hg(CN),.6CAN 22.5
28.5
Mob.
Hg(CNJi
t*. per 100 Mob. S<did Phase.
9
II
12.2
13
13. 5
14.5
16.5
20.5
CM
7.1
8.7
10.4
II. 3
12.9
13 8
15.8
15-9
Hg(CNJj+
Hg<CN),.aCAN
M
M
32
38
42
46
53
54
QH
17 3
18.4
19.3
20.6 •*
22.3 «
23.7
25.3>Hg(CN),.3CiH^
26
M
r.
56
68
70
86
III
122
"5
141
100 gms, pyridine dissolve 64.8 gms. Hg(CN)t at i8^
Mob.
Hg(CN),
per 100 Mob. Solid
.5 26.6 aHg(CN),.3CAN
27. 5 Hg(CN)t.C*H.N
27.7 "
29 «
32
.5 33.8
34.4
38.3
(Schraeder, 1905.)
Solubility of Mercuric Cyanide in Quinoline. (StuookA, x9ta)
Mob. Hg(CN)t
t*. _pa 100 Mob. Solid Phase.
Hg(CN),+CHTN.
45 4. a Hg(CN),.3C,H,N
54 6 "tr.pt 6o*
89(61") 8.2
99(61) 9.2
BSEBCUBT FULBONATE CHgNA.
Mob. Hg(CN),
t*. per xoo Mob. Solid Phase.
Hg(CN),+CH,N.
137 13 . 2 Hg(CN)^aCAN(?)
161 17.4 ««
180 22.5 ••
192 27.1 •
One liter of solution in water contains 0.70 gm. C^HgNiOt at 12* and 1.76
gms. at 49 .
IBBGUBZC lODIDB
(HoUemam, X89&}
Hgl,.
SCH^UBILITY IN WaTBR.
r.
z8
17. s
22
Gms. Hffl, per Liter. Observer.
o . 0004 (oonductivlty method) (KoUzmusch, 1904- os.)
0.040 (BottigoiB, 1884.)
0.054 (Rohbnd, 1898.)
0.0591 . (Mone, X903.)
SCH^UBILITY OF MbRCUROUS IoDIDE IN WaTER AT 25"*. (Sherrill. 1903.)
One liter sat. solution contains 2 X lO"^ gms. Hgsis, 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^
(Hers and Paul, 19x3.)
In Aq. Ball.
Mob. per Liter.
In Aq. Cals.
Mob. per Liter.
In Aq. NaL
Mob. per Liter.
In Aq. Srit.
M(^. per Liter.
Bal,. Hgl,.
0.099 0.059
0.748 0.742
0.978 0.897
X.508 1.462
Cal,. Hgl,.
0.053 0.050
0.252 0.261
0.468 0.440
1.799 1706
Tial.
0.794
1.385
2.225
Hgl,.
0.412
0.622
0.945
Sri,. Hglc:
0.254 0.212
0.355 0.320
0.539 0.582
0.608 0.694
Solubility of
Mob. per Liter.
Mercuric Iodide in
Iodide at 25**. (Sheniii
Gnu. per Liter.
Aqueous Solutions
, 1903; Hen and Paul, 19x3
Mob. per Liter.
OF Potassium
Gms. per Liter.
U. Hgl..
0.05 0.025
O.IO 0.05
0.20 O.IO
0.50 0.25
KI. Hgl,.
8.3 II. 4
16.6 22.7
33-2 45 4
83 113 -6
KT.
I
1.5
2
2.5
Hgl,.
0.50
0.75
I
1.25
' KI. Hgl,.
166 227.2
249 340.8
332 454.5
415 578
Data for the distribution of mercuric iodide between aq. KI solutions and
benzene at 25** are given by Sherrill, 1903.
4^5
MERCURY lODIDB
Equilibrium in the Ternary System Mercuric Iodide, Potassium
Iodide, Water at 20° and 30''. (Duimiagham 1914)
Results at 20
0
«
Results at 30**
•
Gms. per ]
[oo Gms. Sat. Sol.
Solid Phase.
Gms. per zoo Gms. Sat. Sd.
Solid Phase.
KI.
Hgl,.
KI.
Hsle.
SO. 9
193
KI
60.6
• • •
KI
44-4
32.4
f<
40
S3
"+KHrt
39
48
u
39-6
52-7
KHA
37-4
53-6
"+KBtf,
40
52-2
M
•
37.8
52.6
KHgI«
40.2
51-2
M
35-1
52.2
M
39-3
50.3
U
35. 5
SI 2
KHgl^H^
33-7
49.8
U
26.7
503
"+H«It
33
52
M
36.6
49-4
Hgl.
31-4
Si-7
KHglfJtf)
23-7
40.2
M
29.1
52.2
If
14.9
22.5
M
Equilibrium in the Ternary System Mercuric Iodide, Potassium
Iodide, Ethyl Ether at 20^. (Dunningham, 19x4.)
Two liquid layers with compositions as follows, are formed:
Gms. pv zoo Gms. Upper Layer. Gms. per loo Gms. Lower Layer.
Hglt.
2.8
KI.
I.I
I.I 2.4
0.8 2.5
None
Solid Phase.
KI. Hgl,.
None
176 53.2
16.5 56.1
17 58.2.
Data are also given for the four component sjrstem, Hgli + KI + (C|H|)tO +
HiO at 20^ The results are of special mterest since 3 liquid layers are formed.
Solubility op Mercuric Iodide in Aqueous Ethyl ALcoHorr-
KI+KHsIi
KHg]^
Hgl.
KHg]^+HgI«
At I8^
(Bourgoin.)
At 25°.
(Herz aod Knodi — Z. anorg. Ch. 45, 966, '05.)
SolTent.
Abs. Alcohol
11,0+80% 90*^ Ale.
H,0+io%9o® Ale.
Gms. Hglt
per liter.
11.86
2 857
0.086
Wt.% Alcohol Hgl» per 100 cc. Solution. Sp. Gr. of
insolvent. IdilUmols. Gnuns. ' Solutions as V^
100
95.82
92.44
86.74
78-75
67.63
3.86
2.56
1.92
1.38
0-93S
0.45
1-754
1. 162
0.873
0.623
0.425
0.204
0.8033
0.8095
0.8154
0.8300
0.8465
0.8721
Solubility of Mercuric Iodide in Aqueous Methyl Alcohol and in
Aqueous Ethyl Acetate at 25°. (Hers and Anders. 1907.)
In Aq. Methyl Alcohol. In Aq. Ethyl Acetate.
Gms. Hg^
Wt.%
CHpBTi
Solve
m
Ivent.
47 06
64
78.05
100
rfy of
Sonrentv
0.9186
0.8800
0.8489
0.7879
imm o£
Sat. Sol.
Gms. Hglt
per xoo cc.
Sat. Sol.
Wt. % CHr
COOCH,
in Solvent.
</y of
Sat. Sol.
per xoocc
Sat. Sol
0.9187 0.044 4.36 0.9973 0.013
0.8834 0.158 96.74 0.9063 1.87
0.8519 0.445 100 O.9OII 1.09
0.8155 2.590
100 gms. sat. solution in 95% alcohol {dn = 0.8126) contain 0.72 gm. Hgli
at o*, 1.06 gms. at 25** and 2.15 gms. at 50°. (Rcinders, 1900.)
IBBCURIC IODIDE
426
Solubility of Mercuric Iodide in Alcohols.
Alcohol.
Methyl
tt
l<
Ethyl
If
ti
li
it
Propyl
Amyl
tt
tt
Isopropyl
Isobutyl
Fonnuk.
CHiOH
tt
tt
tt
CHiOH
tt
tt
tt
tt
C»H^H
ti
CiHuOH
tt
tt
it
(CH,),CH.OH
(CH,),CHCHiDH
15-20
19
19- S
23
66 (b.pt)
15-20
18
19
19. 5
25
78 (b. pt.)
15-20
19
13
71
100
133.5
81 (b. pt)
22.5
105-107 (b.pt.)
Sp. Gr. o£
799
810
803
816
Gms.IIgIfper
100 Gms.
Alcohol.
3.24 (RoUaod.)
3 . 7 (Timofdew.)
3.16 (de Bruyn.)
3.98 (Beckmaim.)
6.512 (Sulc)
1.42 (RohbuuL)
1.48 (Boufsoin.)
1 . 86 CTimofdew.)
2 . 09 (dc Brusm.)
2 . 19 (Hen and
4.325 (Suk.)
0.826 (RohUad.)
Z.25 CTuBofcifw.)
0 . 66 (Laucanaiki.)
3.66
S.30
9.57
2.266 (Sole.)
0.51 (TimoCeiBW.)
2.433 (Sole)
.)
SOLUBH^ITY OF MERCURIC lODIDE IN MIXTURES OF ALCOHOLS AT 25^.
(Hen and Kuhn, 1908.)
In CHiOH+CiHiOH. In CHtOH+CHjOH.
Percent
CHfOHin
Solvent.
O
4.37
10.40
41.02
80.69
84.77
91.25
ZOO
d[y of
Sat. Sol.
0.8038
0.8039
0.8046
0.8077
O.813I
0.8140
0.8146
0.8156
Gm«.HgI| Percent
per zoo oc. CaHiOH in
Sat. Sol. Solvent.
JyOf
Sat.SoL
0.8156
1.80 O
1.93 II. II
2.08 23.80 0.8155
2.32 65.20
2.89 91.80 O.81OI
2.96 93.75 O.81IO
2.98 96.60 0.8108
3.16 100 O.8116
In CHTOH+CHiOH.
Gms. Hgl| Per cent 4 of ^°^- ^A
perioooc. (VHiOHtn _ ^, perzoocc
Sat.SoL Solvent. Sat. Sd. Sat. SoL
3.16 o 0.8038 Z.80
8.1 0.8036 1.73
3.04 17.85 0.8043 1.65
56.6 0.8057 1.55
1.69 88.6 ... •. •
1.67 91.2 0.8099 1.52
1.53 95.2 0.8108 1.44
1.42 100 0.8116 1.42
Solubility of Mercuric Iodide in Acetone in Ethyl Acetate
AND IN Benzene.
IMM. v«ia. wy
»/• »»05, y«.#
In Acetone.
In Ethyl Acetate.
In Benzene.
Gms. Hgis
Gms. Hgh
Gms. Oclt
per 100 Gmi.
t*. per 100 Gms.
t*.
per 100 Gms.
cSbCOOCsHi.
t*.
(CHa)sCO.
CsHa.
I 2.83
—20
1.49
IS
0.22
18 3.36
+ I7-S
1.56
60
0.88
as 2.09 (K- and McE.)
21
1.64
65
0.9s
40 4-73
40
2-53
84
1.24
58 6 .07
55
319
80 (iMit-) 0.835 (SokO
56(b.pt.)3.a49(Siik.)
76
4.31
74-78 (b.pl.) 4 . 20 (SuIcO
4^
2BBCUBY lODIDC
100 gms. acetone di
SSQ
" benzene
" chloroform
" acetone
II tt
" ethyl acetate
dissolve 2.04 gms. Hgli at 23^ (Beckmaim and Stock, 1895-)
" 0.25 " ^
0.07
2
3.09
147
II
II
II
It
u
u
(red) at 25^
(yellow) at 25**.
at I8^
(Reinden, 1900.)
It
(Naumann, zgza)
One liter sat. solution in benzene contains 2.24 gms. Hgit at 25**.
(Ab^gg and Sherxill, 1903.)
Solubility of Mercuric Iodidb in Aniline.
(Peaice and Fzy, 29x4.)
Gms. HgIt
Gnis.HgI^
r.
per xooGms.
Aniline.
Solid Phase.
V.
perxooGms.
Aniline.
Solid Phase.
-11.48*
. . . CtH«NU|+HgI«.3CANB^
48.8
128. 1
HgltCmO
- 6.S
23-35
HgIs.aQH|NH|
63.6
163.8
M
+ 0.4
28.69
it
70.82
184. 1
M
17.8
42.85
u
76.2
201.6
M
21. 1
47 55
u
95-9
246.7
M
26.9
SS- 47
u
io8t
'• • •
" +H«I^ (yellow)
30.1
62.05
«
"5-7
281.8
^gI, (yellow)
36.2
75.80
M
137-2
285.2
«<
42.9
049
M
181. 1
297.9
M
46.8t
• • •
" +HgI,(ied)
199. 1
863.2
«
Eutec.
t Tr.pt.
Additional data on this system are also ^ven by Staronka, ipio.
Data for the solubility of mercuric iodide in nitrobenzene and m p nitrotoluene,
determined by the synthetic (sealed tube method) , are given by Smits and BaJc-
horst (1015). The transition point of Hglj, red to yellow, was found to be at
1.68 mol. per cent HgIt and 127.5^ in nitrobenzene and 1.81 mol. per cent Hgli
and 128*' m p nitrotoluene. The interesting part of the investigation is tne
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,
usins^ a Beckmann apparatus, are given by Mascarelli (1906a;. Observations
on the appearance and color changes of the Hgli are given.
Solubility of Mercuric Iodide in Carbon Disulfide.
(Linebazger, 1894; ArctowsU, 1894, 1895-96.)
f.
Gms. Hgl^
per 100 Gms.
Solution.
r.
Gms. Hell
per 100 (Tms.
Solution.
r.
Gas. Qgl^
per zoo (^in.
Sokition.
116
93
86.5
10
0.017
0.023
0.024
0.107
- 5
0
+ 5
10
O.14I
0.173
0.207
0.239
15
20 •
25
30
0.271
0.320
0.382
0.445
One liter sat. solution of mercuric iodide in CSs contains 3.127 gms. at 15^ '
(Dawson, zqo9b).
One liter sat. solution of mercuric iodide in CCU contains 0.170 gni. at 18 .
(Dawson, z9o9b.)
Data are also given by Dawson for the distribution of Hgis between aqueous
solutions of KI and CSs at 15^ and aqueous solutions of KI and CCU at 18**.
100 cc. anhydrous hydrazine dissolve 69 gms. HgIs with precipitation of Hg
at room temp* CWelsh and Biodecsoo. 19153
MERCURY lODm
4a8
Solubility of Mbrcuric Iodide in Sbvbral Organic Solvents.
(Sulc — Z. uioix. Ch. 2S» 40Z1 '00.)
SolTent.
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
Efexane
FonnuU.
CHCl,
CHCl,
CHBr,
CC1«
CCl,
C^,Br
QH,I
(CHj),.CHCH,Cl
HCOOCH,
HCOOCjH,
CHjCOOCH,
CH,CH(OC,H^
CH,.O.CH.Cl4ca
t».
i^-ao
61 (b. pt.)
18-20
18-20
75 (b- pt.)
18-20
38° (b. pt.)
18-20
i8-ao
85.5° (b. pt
69
3^-38
5^-55
56-59
105
117
67
<l
it
(C
M
u
Gms.Hglsperxoo
Cms. Sotvent.
0.040
0.163
0.486
0.006
0.094
0.643
0.773
0.748
2.04Z
) i.aoo
0.328
1. 166
a. 150
a. 000
6. 113
0.072
Solubility of Mbrcuric Iodide in
Iodide.
In Ether.
(Sulc; Luxcynskl.)
A* Cms. Hgli per xoo
* ' Gms. (CA^.
o 0.62
36 0.97
35 (b. pt.) 0.47 (Sulc)
Ethbr and in Mbthylbnb
In Methylene Iodide.
(Retfen — Z. anocg. Ch. 3, 853, 'gsO
IS
100
180
Gmi. Bghper loe
Gmf . CH>Ia.
a-S
16.6
58.0
Solubility of Mbrcuric Iodidb in Patty Bodibs.
(Mehu — J. pharm. chim. [^ la. 949, '85.)
av Gnu.
' * xoo Gms
Hell per
is.SolYeiit.
0.5
13
4.0
90 .0
1-3
OQIfCllt.
Bitter Almond Oil 25
Bitter Almond Oil 100
Castor Oil 25
Castor Oil 100
Nut Oil zoo
100 grams oil of bitter almonds dissolve 5.0 grams HgIs.KI at 2^.
SoLUBiLrry of MBScenc Iodidb in Oils.
(Anon, I9Q3. Z904.)
Solvent.
Vaseline
Vaseline
Poppy Oil
Olive on
Carbolic Acid 100
Gnu. Hcis
100 Gms. SolVienl
as
0.025
100
0.20
as
i.o
as
0.4
100
a.o
Gmi. Hgl|
Gms. HA
00.
1
per 100 oc
OU.
oo.
perioooc
OiL
Castor Oa
1.90
Peanut Oil
0.52
Walnut "
1.29
OUve "
0.4s
Linseed "
1.23
Almond "
0-39
Cod Over "
OS4S
Vaseline
0.d6
429 2BBCUB7 IODIDE
SoLUBiLmr OF Mbrcuuc Iodide in Pyudinb.
(Determinations from —50^ to oS.s'* made by saturating the solvent at con-
stant tenvseratures are p;iven by Mathews and Ritter (1917;. Measurements of
the points of solidification of various mixtures of the two components, covering
the range from 10^ to I35^ are given by Staronlca (1910).
Gii».Hgl«
Cms. Hiili
f.
periooGms. Solid Phaae.
f.
per 100 Gnu. Solid Phase.
Sftt. Sol.
Sat.SoL
-so
1.93 HgI|.aC,H,N
90.08
61.43 HA.3CAN
-31.5
4.27
If
100
65.72 «
— 10
10.28
M
105
6S.89 "
— O.I
14 85
<l
107 m. pt.
72.09 «*
+ 8.83
18.42
M
105
75.67 -
20.02
24.40
«
100
79.73 «
^SSS
27.90
M
90
84.16 «
40.08
37.64
U
87 Eutec.
85.17 «+HgI..(»N
50.02
43 IS
M
100
86 HgIt.QH|N
60.07
48.29
U
120
87 . 16
80.05
57.60
M
13s
88.78
Solubility
OF Mbrcuric Iodidb in
(StaiODka, 1910.)
QXJINQLINB.
r.
periooMols.
Solid Phaae.
f.
I Mols. BmV
'jxr 100 Mob. ' Solid Phase.
•
100
4.7
;HgI..aCAN
160
37 . 7 HgI..CAN
i^S'S
. 91
tt
165
41.6
133 -5
132
M
165
43
138
23.1
ft
170
48.8
I4S
26.7
Hgli-CHTN
169.5
49-5
IS3
31 -4
<i
166.5
544
153 31.4 AUU.5 54.4
Fusion point data for mixtures of Hgli + I are given by Olivari, 1908.
MERCURIC lODIDC Diamine (NH,),HgIs.
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 tlmn 48 gms. NH| per liter.
2BRCUR7 NITRATE (ic) Hg(NO,),, (ous) Hg,(NO,)s.
TOO gms. anhydrous lanolin (m. pt. about 46°) dissolve 1.15 gm. Hg(NOi)t
at 45**. (Klose, 1907.)
^ 100 cc. anhydrous hydrazine dissolve about 2 gms. Hgi(NOt)s with precipita-
tion of Hg at room temp. (Welsh and Biodenon, 19x5.)
2BRCURT OXIDE HgO.
Solubility in Watbr.
(Schick, 1903.)
Gms. per xooo cc. SoIutfoD.
■ A
25 0.05x8 yellow HgO 0.0513 red HgO
100 0.410 yellow HgO 0.379 red HgO
At 25* the mixtures were constantly agitated for 4 days or longer. At lOO*
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 HsO dissolves 0.05 ^gm. HgO (red, large grains) at 25^. (Hulett, 1901.)
One liter H^ dissolves 0.15 gm. HgO (red, finest grains) at 25^ "
mEcuBY oxm 4^0
Solubility op Mbrcusic Oxidb in Aqubotts Htdsofluoric Acm at 25^
VonotXty
Gins.Qgper
Gm. Atoms Bk
of HP.
9.60c. Sit. SoL
perUter. •
0.12
0.0242
0.01258
0.24
0.047s
0.0247
0.57
O.I2IO
0.0629
I. II
0.2247
O.II68
2.17
0.4976
0.2586
imtCUBT DiPHlNTL Hg(CA)t.
Fusion-point data for mixtures of Hg(CtHi)t + Sn(CcHf)4 are given by Cambi
(1912).
MERCURY ttLBNin HgSeOk.
S(x.UBiLiTT IN Aqueous Sodium Sblbnttb Solutions at 25^
(Rosenheim and Pritze, 1909.)
Normality Cms. HgSeO^
of NaaSeOk per 100 Cms.
Sdutioo. Sat. SoL
0.0625 0.18
Normality
Gms.HgSeOb
NaJSeQiof
perzooGma.
SaLSoL
OS
0.70
I
1-39
2
2-73
0.125 0.32
0.2s 0.53
MERCURY SULFATE (ic) HgSOt.
Equilibriuii in thb System, Mercury 'Oxidb, Sulpur 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 35°.
Results at so"".
Uquid.PhaM
!.
Solid Phase.
Liquid Phase
•
Solid Phase.
tifi.
S(V
H«0.
H,0.
SQ|.
HgO.
^i^^fanA A Um^Cm
98s
1.34
0.33
sHg0.S0b
98.9
0.96
0.17
3H80.S0b
96.6
3.49
0.92
<«
96
3.05
0.93
M
94-4
3-93
i.6s
M
93-2
4.92
1.90
M
93-9
4.34
1.85
2.12
3Hc0.S0^and
92.8
5. 10
2.09
M
94-4
4-52
3Hc0.3S0b.aH^
92.8
5. 16
2.q6
M
93-4
465
1.94
iBtQ.iSOt.2Hfi
92.5
5.34
2.12
M
93.9*
93.9
4.81
5"
2.29
1.98
3Hg0.S0b
3HsO.3SQ|.3H|0
92.2
557
2.20 1
3Hc0.S0band
3Hc0.sS0b.a^0
92 -3*
5. 30
2-54
aHgCSQi
92.1
5-75
2. II
3Hg0.sS0b.sH^]
92.3
5-58
2.09
3Hg0.aS0k.aH^
92
5.80
2.16
(i
93.1
91.9
S-8i
S-97
2.08
2.90
iHgO'SOt
91.2*
6.27
2.56 j
3H«0.S0band
EgOJSOi
91.9
91 -3
6. IS
6-54
2.05
2.13
5Hg0.3S0b.3H^
91 5
6-34
1
2.19
3HcO.3SQ1.3H/>
andHgO.SQi
91.3
6.77
2.02
Hg0.S0^H/>
91 -3*
6.37
2.30
B«O.S0b
91 -3
6.90
1.80
M
91.6
6.69
1.75
M
91 -3
7.67
1. 01
11
91. 1
8.32
O.S7
«
91-3
7.84
0.89
H80.S0b.H«0 and
90.5
9. II
0.4
«
91
8.36
0.69
Hg0.S0b
89.6
10.2
0.23
«
90s
8-. 95
0.53
M
86.7
l$'2
0.06
«
89.3
10.6
0.22
H80.S0b
316
68.4
0.03
m
75-8
34.3
trace
«(
39-3
60.7
trace
««
■
* Indicates uniUble equilibriiun
431 MEBCUB7 8ULFATB
MBBCUB0U8 SULFATE Hg,S04.
Solubility in Water, in Sulfuric Acid and in Potassium Sulfate at 25*.
(Dnicker, 1901; Wright and Tbomioo, iSSi-^Ss; Wilamore, 1900.)
Sd«nt. . Hg.SO.perLtor.
I Gm. Md. Gbis.
Water 11.7110"! 0.58 (•.47 W. and T., a39 WJ
Aq. H2SO4 ( 1 .96 gms. per liter) 8.31 " 0.41
Aq. HsS04 ( 4 .90 gms. per liter) 8 . 78 '' 0.44
Aq. H2SO4 ( 9.80 gms. per liter) 8.04 '' 0.40
Aq. E«S04 (34.87 gms. per liter) 9.05 " 0.45
Solubiltty of Mbrcurous Sulfate in Water at Different TEiiPERATURES.
(Barre, 191 x.)
Gms. per xoo Gms. Sat. Sol.
f. , ' . SoUd Phase.
HgsSOi. HtSOi.
16.5 0,0$S 0.008 HbS04
33 0.060 0.018
50 0.065 0.037
7S 0074 0-063
100 0.092 0.071
The mixtures were kept at constant temp, but not constantly a^tated. By
successive treatment of a given amount of HgtS04 with HiO, it is gradually
converted to an almost insoluble basic salt, HgtO.Hg1SO4.H1O.
S(H«UBILITY OF MeRCUROUS SULFATE IN AqUEOUS POTASSIUM SULFATE
Solutions. (Bane, 191Z.)
Results at i$\ Results at 33''. Results at 75^[
Gms. per loo Gms. Sat. Sol. Gms. per loo Gms. Sat. Sol. i Gms. per xoo Gms. Sat. SoL
if
«
u
M
-* \ / * . \ <•
KtS04. HgiS04. H«S04(fiee). KiSOi. Hg|SO«. HtSOtCfxee). K<S04. HftSOli. H«SO«(free)
2.90 0.0475 o.ooiBo 2.94 0.0677 0.0250 3.10 0.1344 0.1684
5.70 0.0703 0.0093 5-68 0.1015 0.0350 5.75 0.2120 0.2135
8.22 0.0912 0.0098 8.30 0.1364 0.0441 8.50 0.2951 0.2514
8.77 0.0994 ••• 10.70 ©.'1724 0.0438 13.20 0.4610 0.2503
9.44, '0.1080 o.oiio 11.90 0.1902 0.0420 17.30 0.6440 0.2225
2BBCUB7 SUUIDE HgS.
One liter HtO dissolves 0.054 >< i<^ mols. HgS » 0.0000125 V^' at I8^
(Weicel, 1906, 1907. See also Bruner and Zawaddd.)
Hexamethyl IHLLITIC ACID Ester C«(COOCH,)«.
Data for the ternary system hexamethyl mellitic acid ester, phenol and water
are given by Timmermans (1907).
MINTHOL CioHi/DH.
One cc. of 95% alcohol dissolves about 5 gms. menthol at room temp.
(Greenish and amith, X9Q|3«)
Freezing-point Data (Solubility, see footnote, p. i) are Given for the
Following Mixtures.
Menthol + Ethylene bromide (Dahms, 1895.)
" + Menthane (Vanstonc, 1909.)
" 4- Methyl urethaa (Scheuer, 19x0.)
" 4- Naphthalene "
" +p Toluidine (Pa^riawiki. 1893)
SoLroiFicATiON Points of Mixtures of Menthol and Salol. (B«iiucd,x9xa,x9i3-)
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
432
CH4.
SOLUBILITT IN WaTBR.
(Winkler, 1901.)
f.
».
/J'.
«.
f.
/).
r.
«•
0
0.05563
0.05530
0.00396
40
0.02369
0.02198
0.00159
S
0.04805
0.04764
0.00341
SO
0.02134
0.01876
0.00136
10
0.04177
0.04127
0.00296
60
O.OI9S4
0.01571
0.00115
IS
0.03690
0.03628
0.00260
70
0.01825
0.01265
0.00093
20
0.03308
0.03233
0.00232
80
0.01770
0.00944
0.00070
25
0.03006
0.02913
0.00209
90
0.01735
0.00535
0.00040
30
0.02762
0.02648
0.00191
100
0.01700
0
0
For the values of B, ff and
Q see Ethai
ie,pai
ee285.
Solubility of Mbthanb in Methyl Alcohol and in Acetonb.
(Levi, 1901, 190a.)
In methyl alcohol / (Ostwald expression, see page 227) « 0.5644 — 0.0046 1 *
0.00004^.
In acetone / (Ostwald expression) » 0.5906 — 0.00613 / — 0.000046 ^.
From which are calculated the following values:
In Methyl Alcohol.
In Acetone.
f.
I.
t". 1.
f.
I.
f.
1.
0
0.5644
40 0.3164
0
0.5906
40
0.2718
10
0.5144
SO 0.2344
10
0.5247
50
0.1691
20
0.4564
60 0.1444
20
0.4496
60
0.057^
30
0.3904
70 0.0464
30
0.3653
Solubility of Methane in Several Alcohols and Other Solvents.
(McDaniel, 191X.)
Bunaen
Coef.j9(f
Solvent.
Alcohol:
Methyl (99%)
f.
Abs. Coei.
A.
Solvent.
f.
Abs. Qad.
A,
Bunaen
Cod.fi.
It
u
u
Ethyl (99-8%)
«
<«
Isopropyl
ti
u
Amyl
Benzene
«
it
u
Toluene
it
<«
u
ti
22.1 0.4436 0.4103 Toluene
30.2 0.4278 0.3883
40 0.3938 0.3436
49.8 0.2695 0.2278 m Xylene
22.2 0.4628 0.4282
30.1 0.4503 0.4051
40 0.4323 0.3771
21.5 0.4620 0.4275 Hexane
29.9 0.4532 0.4081
40 0.4400 0.3837
60.3 0.4244 0.3478
22 0.4532 0.4196 Heptane
30.1 0.4444 0.4002
22.1 0.4954 0.4600
35 0.4484 0.3976 Pinene*
40.1 0.4198 0.3661
49.9 0.3645 0.3081
25 0.4852 0.4450
30 0.4778 0.4300
• b. pt. iss-i6o*.
ti
ti
it
it
it
tt
a
a
u
40.
SO.
60
21.
30.
50
60
22.
40.
49-
60
22.
30.
40
20
30.
39.
45
55.
1 0.4675
2 0.4545
0.4502
1 o. 5146
5 0.5028
0.4972
0.4870
2 0.6035
2 0.5320
7 0.5180
0.4964
2 0.7242
I 0.6906
0.6675
0.4888
I 0.4620
1 0.4472
0.4440
2 0.3694
0.4080
0.4013
0.3690
0.4778
0.4529
0.4203
0.3992
0.5585
0.4639
0.4380
0.4068
0.6720
0.6221
o. 5820
0.456s
0.4163
0.3914
0.3811
0.3076
Abs. coef. A » vol. of methane absorbed by unit vol. of solvent at temp
8tat^.
For definition of Bunaen abs. coef. fi see carbon dioxide» p. 3270
433
»
Solubujtt of Mbthanb in Ethyl Alcohol.
(Bunaen, 1877, xSQaO
II*.
IdTHANX
t*. a*. 6.4*. "•. IS*' X9*. 13. s*.
Abs. coef. i9 (found) 0.51721 0.50382 0.49264 0.48255 0.4729 0.4629
from which the following fonnula was calculated.
Bunsen abs. coef. fi for methane = 0.52274^5 — 0.00295882 t — 0.0000177 ^•
' The solubility of methane in aq. HtS04 (ChnstofF, 1906) in terms of the Ostwald
solubility expression Ik. In 95.6% HtSOi, ^ » 0.03303; in 61.62% H1SO4,
Ik = aoi407; in 35.82% HiS04, Ik - 0.01815; in HA /« - O.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 lo**. (Christoff. X911.)
The coef. of absorption fi (Bunsen) of methane in petroleum. (Russian) is 0.144
at 10^ and O.131 at 20°. (Gniewoas sod Walfias. 1887.)
Fusion-point data are given for diphenyl methane + naohthalene by Miolati,
(1892) and for diphenyl methane + phenol by Paterno ana Ampola (1897).
Triph
lenyl IHTHANE CH(CeHi),.
Solubility
IN Anilinb.
(Hartley and Thomas, 1906.) J
By synthetic method, see page 16.
Cms.
Gms.
t*.
CH(C8H5)s Mol.per
per xoo cent
Gma. So* CH(C«Hi)s
hitioQ.
Solid
Phase.
•
(
CH(CflHB)i Mol. per
per xoo cent
Gms. So. CH(CsHi)s.
lution.
SoKd
Phase.
23.0
5-4 1.85
CH(CaHi)i.C6HiNHb
rhombs
71 -3
67.9 44.6 CH(C.H.)..C^UNHj
35-3
9-5 3-8
M
71.6
71.7 491
M
43 0
13s S-6
M
71.2
76.3 li'-^
M
521
21.9 9.7
M
70.6
783 57-9
M
61.4
36.5 17.8
M
71.6
82 . 1 63 . 5 CH(r4H|)i mooodinic
66.0
47.2 25.4
M
74-3
84.9 68.2
M
68.7
54.8 31.6
«
82.1
91. 7 80.9
M
70.1
64.6 40.9
«
873
96.1 90.2
M
Solubility
OP Tri Phbnyl Mbthanb in Bbnzbnb.
(Linebarger — Am. Oi
. J. iSi 45. 'm.)
(Hartley and ThomasJ
Gms.
GBas._ w_i
t\
CH(GA)Bper
100 Grams
Solid Phase.
^0 CH(CA)t percent Solid Phaat.
. * • per 100 Gms. pfivVuH V *>«■» *^»»— •
Solution. CH(CtH»)8.
3.9 3.90 CsHe+ CH(C6H.),.C»
33
12.6 4.4
CH(C|H«)>.C&
rhombs
4-
0 4.06 CH(CA)a.Caie
49.4
24.0 8.8
M
12.
S S18
M
65 .6
38.9 17.2
M
16.
1 6.83
M
73-3
S7S 30.2
M
19.4 7 24
M
77.1
674 39-7
a
23-
I 8.95
M
77-9
76.3 SO. 7
*
37.5 10.48 ^^¥^^;asr
77-5
80.2 56.4
M
42.
0 19.61 CH(CsHi)s
76.2
84.1 62.8
M
44.
6 22.64
M
74.6
87.5 69.1
CH(CA)i
monodiBlc
so-
I 30 64
M
76.0
89.0 72.2
•i
sss 40.51
M
78.8
90.5 75-3
•4
71-
0 140.00
M
82.3
93.1 81.3
M
76.
2 319-67
«•
86.6
95.7 87.8
M
Hartley and Thomas call attention to the inaccuracy of Linebarger's results and
to the correctness of the determinations of Kuriloff (1897a). According to
Kuriloff the tr. pt. (CeH6),CH.C6Hi -f CeHe is at 4.2*' and 1.25 mol. % (CeHOiCH.
the m. pt. of (C«Hi),CH.CeHe is 78.2° and the tr. pt.(CeHs)iCH.C«He+ (C«Hi)s.CH
is at 74^ and 69.4 mol. % (C«H5)|CH. ^
Triphenyl IHTHANE
434
Solubility op Tri Phenyl Methane in Carbon Bisulphide.
(Etard — Ann. chim. phys. [7] a» 5701 '94; below— 8o^ Arctowski — Z. anois. Ch. iz» 873, '95.)
Gnu. CH(CA)a
t*. per 100 Gma.
Solution.
— 113.5 0.98
— 102 1.24
— 91 1.56
— 83 I. 91
— 60 3.4
Cms. CHCCeHsH
t^. per xoo Gms. t^.
Solution.
-40 7.5 40
-20 13.7 SO
o 25.8 60
+ 10 38.7 70
20 43-2 80
30 Sa-9
Gms. CH(C6HiJto
per 100 Gms.
Solution.
63-7
72.4
78.6
85 r6
92.3
Solubility of Tri Phenyl Methake rv Hexane and in
Chloroform. (Eucd.)
Gmt. OBKCsHs)^ per xoo Gms.
-30
— 20
— 10
O
+ 10
20
Heacane.
1.3
1.6
3.3
5-6
8.3
Solution
Gms. CH(C«Hs^ per xoo Gob.
Sdution in:
QUorofonn*
10.5
19.0
23 S
28.9
3SO
4IS
30
40
SO
60
70
80
90
Hezane.
12-5
20.0
25.8
45-7
62.0
78 s
97 o
Chlarofonn*
48.8
56.1
63.8
71.7
79.8
87.2
Solubility op Tri Phenyl Methane in;
(Hartley and ThomasO
Pyrrole.
Gms. Mol.
^o CH(C8H^ per Solid
* periooGms. cent Phase.
Sol. CH(C6H«)g.
246
29. 0
31 S
36.8
42.7
46.9
53-2
60.0
63 9
68.5
71. 1
80.0
89. 2
24 -3
29.8
33-4
40.6
49.1
56.0
63 -9
72 -3
76.7
81.9
84.4
91 S
97.6
8.1
10.4
12. 1
15.8
20. 9
25 9
32.8
41.8
47-4
59-8
74.8
91.8
CHCCsH^-CANH
rnombs
CHCCbHb), ,
„ monofiinir
■7
5
5
4
25
33
44 o
47-6
^
57
57-6
62.7
67.0
67.2
74.2
79 o
87.2
Thiophene.
Gms. Mol.
CHCCeHi), per
per too Gms. cent
Solution. CH(C«HB)t.
26.0 10.8
311 135
43-6 21. 1
48.4 24.4
587 329
70. 2 44-7
74.8 50.6
78.7 560
81.9 60.8
82.1 61.3
87.4 705
903 763
96.2 89.9
Solid
Phase.
CH(CbHi)|.G«]EUS
u rhomu
CH(C»Hi), ,. ,
monoauie
u
F.-pt. data for triphenylmethane + naphthalene are given by Vignon (i89i).
Solubility of Triphenyl Methane in Pyridine. (Harti^ and Thomas, 1906.)
Synthetic method used, see note, p. 16.
^ CH(Qft), Mol. per
"^sJSiSr- CH(CH.),.
22 CH(C«H«)|
27 • 2 " mcmodinic
SoUd Phase.
f.
Gms.
CH(C.HO,
Mol. per
cent Solid Phase.
22.8
31-7
37.9
48.7
53-1
46.2
53-3
57-6
66.6
70.1
per xoo Gms. rxxtrxx \
Solution. CH(C.H«),.
59-3 75-6 50-3 CHCCA).
30-7
39-5
43-5
<(
67.8
72.8
80.6
86.8
81.9
85.7
91. 5
95.8
59.7
66.4
77.2
88.1
435 Sulfon
Ethyl and Methyl Sulfon METHANES.
Sglubility in Water and in 90% Alcohol.
r.««.«w«.t«<1 Fi^rmnU *• GlPS. Ccipd. pCT lOO CC.; A.«*lw»?Hr
Water. 90% Alcohol
Sulfonal (CHt)iC(SO|CsHi)t 15 .5 0.22 l . 25 (Greenish aod Smith, 1903.)
Tetronal (CiH»)iC(SOtCsHft)s 15-20 0.18 8.33 (Squire and Gaines, 1905.)
Trional (CH,)(CiH»)C(SOiCiHi)i 15-20 0.31 9.0
U U M
DlSTRIBimON BETWEEN WaTBR AND OlIVE OiL AT RoOli TEMP.
(Baum. 1899; M^y«, 1909.) ^ ^ ,
Gna. Cmpd. per 100 cc Ratio
Compoiind. ' Fonnola. H^ Layer Oil Layer ii
(w). ioh (w) *
Dimethyl Sulfon Dimethyl Methane (CHa)sC(SQ|.CHa)t 0.6072 0.0622 0.103
Diethyl Sdfon Methane CH«(S(^CtH|), o. 610 o. 092 o. 151
Sulfonal (CH,),c(SQiC::iHi)s 0.070 0.0686 0.979
Trional (CHa)(CA)C(SOk.CtHa)s 0.0404 0.1646 4.074
Tetronal (Cai{i)sC(S(^.CiHi)s 0.0462 0.1446 3.756
IIETHTL ACETATE CHiCOOCH,.
100 gms. HtO dissolve 25 gms. CH«COOCHt at 22^. (Traube, 1884.)
More recent data for the solubility of this compound in water are given by
(Herz, 1917).
IIETHTL ALCOHOL CH,OH.
Freezing-points of Mixtures of Methyl Alcohol and Water.
(Pickering, 1893; Baum4 and Borowski, 1914.)
Gms.
*•• per^cL SoHdPhue.
Mixtures.
-130 75- 5 I"
-138.5 Eutec. 77 " +CHdOH
— 130 82 GEUOH
— 120 86.5
— no 92
-95.7 100
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, 19x0.) Chloroform and Water. (Bonner, 19x0.)
Composition of Homogeneous Mixtures. Composition of Homogeneous Mixtures.
, , « ^ , A ^
Sp. Gr. of Gms. Gms. Gms. Sp. Gr. of
Mixture. CHC1«. I^. CI^H. Mixture.
0.979 0.021 O.161
1.30 0.90 o.io 0.3s 1. 17
1. 13 0.80 0.20 0.49 1. 12
1.04 *o.73 0.27 0.57
I 0.70 0.30 0.60 1.08
0.97 0.60 0.40 0.70 1.05
0.9s 0.50 0.50 0.77 1.02
0.93 0.40 0.60 0.83 I
0.92 0.20 0.80 0.84 0.97
0.92 O.IO 0.90 0.74 0.96
0.93 0.013 0.987 0.267 0.98
Gms.
Gms.
^0 ch^h
Dcr 100
Cms. Sol.
Solid
^ CHdOH
per zoo
Cms. Sol.
S6M
Phase.
Phase.
-10 14.5
Ice
-70 58.3
Ice
— 20 25
14
-80 62.6
u
-30 33
M
-90 65.7
u
—40 40
<f
-100 68.8
«
-50 47
«i
— no 71.5
f(
—60 52.6
— 120 74.0
<f
«
Gms.
Gms.
Gms.
CCI4.
H/).
CHdOH.
•0.98s
o.ois
0.2IS
0.974
0.026
0.328
0.90
O.IO
0.74
o.do
0.20
1. 10
0.70
0.30
1.40
0.60
0.40
1.68
0.50
0.50
1. 71
0.40
0.60
1-77
0.20
0.80
1.88
O.IO
0.90
1.90
0.026
0.974
1. 04s
IdTHTL ALCOHOL
436
iMisciBiLiTY OF Methyl Alcohol (see Note, p. 287) at o* with
Mixtures of:
Brombenzene and Water. (Bonner. 19x0.) Ethyl Bromide and Water. (Bonne^ 19x0.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
Gms.
CABr.
0.991
0.985
♦0.98
0.90
0.80
0.70
0.60
0.50
0.40
0.30
0.20
0.09s
0.016
Gms.
H^.
0.009
0.015
0.02
O.IO
0.20
0.30
0.40
0.50
0.60
0.70
0.80
0.905
0.984
Gms.
CH,0H.
0.230
0-314
0.40
1. 01
1.50
1.84
2.065
2.24
2.30
2.28
2.20
1.927
I 332
Sp. Gr. of
Mixture.
1.24
• • •
1.04
0.98
0.95
0.94
0.91
0.90
0.89
0.89
0.90
0.91
Gms.
'CH»Br.
0.973
0.950
0.936
0.90
0.80
0.70
0.60
0.50
0.40
0.20
O.IO
0.022
Gms.
H/).
0.027
0.05
0.064
O.IO
0.20
0.30
0.40
0.50
0.60
0.80
0.90
0.978
Gms.
CH«0H.
0.202
0.33
0.393
0.54
0.86
1.04
1. 18
1.26
I-3I
1. 21
0.94
1-94
Sp. Gr. of
Mixture.
1.27
• • •
1. 18
1. 14
I OS
1. 01
0.99
0.97
0.96
0.94
0.94
0.98
MisciBiLiTY^OF Methyl Alcohol (see Note, p. 287) at o* with
Mixtures of:
Hexane and Water. (Bonner, 19x0.)
Heptane and Water. (Bonner, 19x0.)
Composition of Homogeneous Mixtures.
Composition of Homogeneous Mixtures.
A
f
Gms.
Hexane(x).
0.973
Gms.
0.067
Gms.
CHiOH.
4.280
Sp. Gr. of
Mixture.
• • •
r
Gms.
Heptane(x).
0.966
Gms.
H,0.
0.034
Gms.
ch,oh.
4.78
Sp. Gr. of
Mixture.
• ■ •
0.90
0.80
O.IO
0.20
4.69
5-26
0.80
0.80
0.90
0.793
O.IO
0.207
5-55
6.36
0.80
0.82
0.691
0.60
0.309
0.40
5 -710
6.17
0.82
0.81
• 0.70
0.60
0.30
0.40
7 30
8.22
0.82
0.82
0.491
0.40
0.509
0.60
6.365
0.83
0.83
0.50
0.40
0.50
0.60
8.76
8.6s
0.82
0.83
0.30
0.20
0.70
0.80
6.13
5-49
0.84
0.85
0.30
0.198
0.70
0.802
7.78
6.71
0.83
0.84
O.IO
0.016
0.90
0.984
4.01
1.759
0.86
0.91
O.IO
0.038
0.90
0.962
4.40
2.96
0.87
0.91
(i) The hexane and heptane used were Kahlbaum's "aus Petroleum."
100 cc. cotton seed oil (Ji6= 0.922) dissolve 4.84 gms.CH;,OH at 25**.
. (Wroth and Reid, x9x6.)
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, X9x6.)
tMI Layer.
0.199
H|0 Layer.
17.28
Ratio.
86.6
Oil Layer.
0.27s
H«0 Layer.
23.48
Ratio.
85.2
0.253
0.298
0.264
23-34
25-73
24-15
92.2
86.2
91.3
0.258
0.284
24.44
23.06
94
81.4
Freezing-point curves (solubility, see footnote, p. i) are given for the following
mixtures: CHaOH -|- SO,, CH,OH + C,H»COOH, (CH,0H.HC1) +
CjHbC(X)H, (CHiCOOH.HCl) + CH,OH (Baum6 and Pamfil, 1914):
CH,OH 4- NH, (Baume and Borowski, 1914); CH,OH + CH|I (Baume and
Tykociner, 19 14).
437
METHYL AMINES
METH7L AMINES CH,NHs, (CHs)tNH, (CHs)iN.
Freezing-point data (solubility, see footnote, p. i) for mijrtures of CHjNHi -|-
H,0, (CH,),NH + H,0 and (CH,),N + H,0 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:
Amine.
CHJSTH,
(CH,),NH
Vapor Pres-
suiein
nzD. Hs*
40.6
90.3
Ostwald Solu-
biUtyCoef./.
(secp.aa?).
S"
230
BunsenAbs.
Oxi.fi,
(see p. 337).
419
188
Solubility of Trimbthyl Amine in Various Solvents at 25®.
(v. Halbon, 19x3.)
The measurements were made according to the dynamic method in the form
developed by R. Abe^g and his collaborators (Gaus, 1900; Abegg and Riesenfeld,
1902). The calculations of the partial pressures of the trimethy&mine were made
according to the Abegg and Riesenfeld method.
E » calc. partial pressure of (CHt)iN above a i normal solution, based on
Henry's Law.
«
')X » solubility, i.e.. the quotient of the concentration in the solution and in the
, ^ mols. (CH|)aN per liter X RTX 760 „_
gas phase: X = ^. . f rr-u \ kt • iT" t ^^ X 760 = 18,590.
partial pressure of (CHi)tN m mm. Hg ' '^'^^
Solvent.
Methyl Ale.
Ethyl
Propyl
Amyl
Benzyl
Acetone
K
(I
(I
B.
26.1
39-5
39.4
48.3
14.2
243
X.
711
471
472
38s
1308
E.
X.
Solvent.
Acetophenone 321 57.9
Ether 349 53.3
Acetonitrile 292 63.7
Nitromethane 329 56.5
0 Nitrotoluene 340 54. 7
X.
84.S
76.2
WVr V A^«MVVXf>UWM^ 0*f Oft
76.7 Nitrobenzene 350 53.1
Solvent. B.
Ethyl Acetate 220
Ethyl Benzoate 244
Chloroform 31.1 598
a Bromnaphthalene 409 47
Hexane 248
Benzene 172
75
109
Two determinations are also given for triethyl amine:
Xm in hexane » 2160. Xss in nitromethane »= 400.
Methyl Amine and Tri Methyl Amine, Distribution between:
Water and Benzene.
(Hers and Fiadicr — Ber. 38, X143, '05.)
Water and Ani5rl Alcohol.
(Hen and Fisclief Ber. 37f 475^» '04.)
Gnu. NHf(CHa)
MnUmob NHs(CHa)
Cms. N(CHa)i
Millimola
;N(CHt>s
per xoo cc.
per
xo cc.
per xoo cc.
perj
to cc.
Aq. Alcoholic
' Aq.
AlcohoUc'
Aq.
QH* '
Aq.
QH.
Layer. Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
Layer.
0.37 0.12
^•^SS
0.3804
0-34S
0.174
•0.584
0.29s
0.94 0.33
3 036
1.070
0812
0396
1-377
0.670
1-57 0.54
5 054
I -759
107s
OS4S
1. 819
O.92X
1.89 0.69
6.083
2.219
1.462
0.731
2.474
1-237
200 0.72
6.429
2.315
2.139
1. 077
3.619
1.823
2.53 0.92
8.126
2. 981
2-757
I 376
4.663
2.328
330 1.24
10.613
3-974
3.292
1.683
5-568
2.847
3 996
2 053
6.760
3-474
6.582
3-465
"•13s
5.861
METHTL AMINKS 438
Distribution of Mbthylaminb between Water and Chloroform and Di-
methyl AND TrIMBTHYL AmINBS BETWEEN WATER AND TOLUENE.
(Moore and Winmill, 19x2.)
Results at 18**. Results at 25**. Results at 32.35^
»_.- Cm. Equiv. per Partition Gnu Equiv. per Partition Gm. Equiv. per Partition'
^^^'"^ Liter Aq.|Layer. Coef. Liter Aq. Layer. Coef. Uter Aq. Layer. . Coef.
(CH8)NH2 0.0817 8.496 0.1203 7.965 0.1399 S-99
" 0.0809 8.477 0.1312 8 0.0959 6
(CH«)2NH 0.0759 23.28 0.1203 19.013 0.1003 13.38
" 0.0975 23.29 o.ioio 19.05 0.1043 ^3-3^
(CiDsN 0.0688 3.297 0.0677. 2.291 0.1182 1.815
'" 0.0791 3.290 0.0641 2.297 0.1248 1.820
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).
AMDVK HTDBOCHLORIDE (CH,),NH.HC1.
100 gms. HiO dissolve 369.2 gms. (CHs)sNH.HCl at 25^ (Peddle and Turner, 19x3^)
100 gms. CHCU dissolve 16.91 gms. (CH|)»NH.HC1 at 25**.
Phenyl METHYL AMDVK HYDROCHLORIDE (CH,)(C«Hb)NH.HC1.
I00gms.Ht0 dissolve 378.8!gms. (CHt)(CfH|)NH.HClat25^ (Peddk and Tomer, '13^
Di and TriMETHYL ABONE CHLOROPLATINATES, (CH,),NH.HtPtCU,
(CH,),N.H,PtCU.
Solubility of Each in Aq. Alcohol at o^. (Bertheaume, z9za)
Gms. Each Compound (Determined Sepa-
c-iygjj* rately) per 100 Gms. Solvent.
(CH,),NH.H,PtCI«. (CH^N.H,PtCI«.
Absolute Alcohol o . 0048 o . 0036
90** " o.iio 0.070
80° " 0.325 0.243
70° " 0.558 0.391
60** " 0.996 0.766
METHYL BUTYRATE CtHTCOOCHt.
100 gms. HsO dissolve 1.7 gms. CsHtCOOCHs at 22**. (TVaube, X8S4.)
More recent data for the solubility of methyKbutyrate in water are given by
Herz, 19 17.
METHYL BUTYRATE, METHYL VALERATE.
Solubility of Each in Aqueous Alcohol Mixtures.
(Bancroft, 1895; from Pfeiffer, 1892.)
100 cc. H|0 dissolve 1.15 cc. methyl butyrate at 20^
cc. Alcohol
cc. H,0 Added.*
cc. Alcohol
in Mixture.
cc HiO Add
in Mixture.
butyrate.
Valerate.
Valerate,
3
2.34
1.66
27
44IS
6
6.96
S'06
30
52-37
9
12.62
9 03
33
62.25
12
19-45
13-40
36
74-15
IS
28.13
18.41
39
91-45
18
38.80
24
42
00
21
SS-64
30.09
24
00
36.72
* cc. H}0 added to cause the separation of a second phase in mixtures of the given amounts of ethjl
alcohol and 3 cc. portions of methyl butyrate and of methyl valerate respectively.
METHYL ETHER (CH,)tO.
F.-pt. curves are given for (CH|)20 -f H2O (Bauni6 and Perrot, 1914) ; (CHj)jO +
CjH,, (CH»)20 4- SOi (Baume, 1914); (CHa)iO + NO (Baum6and Germann, 1914);
rCHi)tO + CO] (Baumi6 and Borowski, 1914).
439 METHYL lODHUB
IODIDE, Methylene Chlori(fe and Methylene Bromide.
SOLUBILITT OF EaCH IN WaTBR. (Rex, 1906.)
Gms. per xoo Gns. %0.
CHiI. CHtOt. CHtBiv.
o 1.565 2.363 I. 173
10 1.446 2.122 I. 146
20 1*419 2 I. 148
30 1*429 1.969 I. 176
Fusion-point data for methyl iodide + pyridine are given Dy Aten (i905-o6).v
METHTL ORANOE HtNC«H4.Nt.C«H4SOsNa.
100 ems. HiO dissolve 0.02 gm. methyl orange at 20-25^] (Debn, 19x7.)
'^ pyridine " 1.80 "
aq. 50% pyridine " 51.5 "
IIETHTL OXALATE (CH,)tC,04.
joogms. HsO dissolve 6.18 gms. (CHi)tCt04 at 20-25^ (Dehn, 19x7.)
pyridine "j 48 "
aq. 50% pyridine " 931 "
" 95 % formic acid " 22.58 " " at 20.2* (Aachan, 1913.)
F.-pt. data for (CHa)iC|04 + HiO are given by Skrabal (1917).
METHYLENE BLUE (CH,),N.C«H,(NS)C«H,:N(CH|),C1.
100 gms. HtO dissolve 4.36*gms. methylene blue at'20-25*. (Dehn, '17.)
'^ pyridine " o.2er "
aq. 50% pyridine " 0.74 "
Data for the distribution of methylene blue between aniline and water are
given by Pelet-Jolivet (1909).
METHYL PROPIONATE CtH4COOCH,.
100 gms. HtO dissolve 5 gms. CtHiCOOCHt at 22^. (Trftube, 1884.)
* More recent data for the solubility of methyl propionate in water are given by
Herz (1917).
METHYL SALICYLATE CfH40H.C00CH,.
100 cc. HjO dissolve 0.074 gm- C6H40H.C(X)CHi at 30". (Gibbf, 1908.)
100 cc. 0.1 n H»S04 dissolve 0.077 gi"* C6H4OH.COOCH1 at 30*.
Solubility of Mbthyl Salicylate in, Aqueous Alcohol at 25^. (Seidell. 1910.)
wt. %
qiLoH
in Solvent.
V ^f . Gms. CiHiOH.-
Sftt. Sol. j^ Gms. Sat. Sol.
c;H.dH
in Solvent
Q«r Q/»i l-UUt.ni per
»'• ^»- 100 Gms. Sat. SoL
0
Z
0.12
60
0.923 z8.6o
30
0.
958 0.60
6s
0.929 30.50
40
0
940 2.30
70
0.943 3940
SO
0
.925 6.20
75
0.974 58 so
SS
0.
.922 10
80
1.050 72
Solubility
OB
' Methyl Salicylate
IN Aqueous Alcohol at Different
Temperatures.
(SeideU, 1910.)
Wt. % CsH^OH
in Solvent.
Gms. C4H4OH.COOCH1 per
100 cc. Solvent at:
r
A
A A
15 .
»'.
25 . 30*.
0
(about) 0.1
0.1
O.I O.I
30
<?-3
0.4
0.5 0.6
40
0.8
I.I
1.4 1.8
SO
2.4
35
S 6
SS
4.2
6
7.8 95
60
7.7
10
12. 5 15. 5
6s
13
16.5
20.2 24.5
70
22
28
33 40
75
43
52
62 72
80
92
135
z8o 230
METHYL SULFAni' 440
MITHTL SULFATE (CHi),SO«.
Reciprocal Solubility of Methyl Sulfate and Oil of Turpentine.
The determinationi were made by the synthetic method (sealed tubes).
The dn 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^
Gnu. (CHt)«S04 per xoo Gnu.
r.
80
90
ICO
los
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-prdiamidobenzophenone) CO[CeH4(4)-
N(CH,)J,.
100 gms. HsO dissolve 0.04 gm. of ketone at 20-25°. (Delm. 19x7 )
pyridine, " 992 "
" aq. 50% pyridine " 3-59 "
MOLTBDENUM TRIOZIDE (Molybdic acid dihydrate) M0O1.2H1O.
Solubility in Water. (Rosenheim and Bertheim, 1903.)
Gnu. MoOt per looo Gnu. Gnu. MoOt per zooo Gms.
Gnu. (CHa)9S04
per XOO Gnu.
f.
(CH,),S04
.Q«Hm
Rich Layer.
Rich Layer.
30
95
4
40
93
S
so
gi
6
60
91
8
70
89
10
(CHJtSO.
Rich Layer.
lUdiluyer,
87
13
84 •
17
76
27
68
37
f.
c-—- ^^^
Sat. Solution.
H,0.
18
1.065
1.066
23
1.822
1.856
30
2.570
2.638
40
4541
4.761
48
5 980
6.360
50.2
6.431
6.873
54 .
7.283
. 7..8SS
• .
Sat. Solution.
HiO.
59
10. 117
11.258
60
10.760
12.057
66
14 . 730
17.274
70
17.048
20.550
74-4
17.290
20.904
75
17.300
20.920
79 .
17.400
21.064
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 fi 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 Davidaohn, 1903.)
Gnu. MoQi per 1000 Gnu. Gnu. MoOi per zooo Gnu.
t". r -> t*.
Sat. Solution. Bfi. Sat. Solution. Bfi.
14.8 2. 112 2. 117 45 3.648 3.661
24.6 2.612 2.619 52 4.167 4.184
30.3 2.964 2.973 60 4.665 4.685
36.8 3.284 3.295 70 4213 4.231
42 3-434 3 446 80 5.185 5.212
Solubility of Molybdic Acid Dihydrate in Aq. Ammonium Salt
SCH-UTIONS. (R. and D., 1903.)
.. - , Gms. MoQi per 1000 Gms.
• • Solvent. ^ — ^ , . *
Sat. Solution. Solvent.
29.6 10% (NH4)2S04 18.91 19.27
31.5 io%NH4HS04 26.79 27.53
41 -8 " 33.22 34.36
Fusion-point data for MoOs + NajMoOi are'given by Croschuf! (1908).
49-7 36.32 3769
■' Gr
441
Ci7HmNQ|.HiO.
Solubility in Sbvbkal Solvbmts.
(U. S. p.; MQUcr, W.. 1903.)
Solvent.
Gms. Mor^dne per 100 Cms.
Solutioii.
Water
Alcohol
Ether
Ether sat. with
HsO
HsO sat. with
Ether
Benzene
Water
Chloroform
Water
Acetone
Aq. so Vol. %
Acetone
Water
Water
At i8*-aa*.
0.0283
0.013 Z
0.0094
At 25*.
0.030
0.600
0.0224
At8o*.
0.0961
1.31 (6o*»)
0.0447 • • • • • •
0.0625 • ■ • ■ ■ •
0.0254 (20^ (Wintefstein, 1909.)
0.0504 ^20®) "
0.0288 (15**) (Guerin, 1913-)
0.128 (15**)
0.132 (is**)
0.0217 (20^) (ZaUi, 1910.)
0.0192 (20^) (GiiOd. 1907.)
Solvent.
At i8*-aa
Chloroform 0.0655
Amyl Alcohol
Ethyl Acetate o.z86z
Petroleum
Ether 0.0854
Carbon Tetra-
chloride
Qua. MoKphiiM per 100 Giiis»
Solution.
Glycerol
CCI4
Aniline
Pyridine
Piperidine
At as\
0.0555
0.8810
0.1905
0.032 (17*)
Diethylamine 7.41 (20^)
50% Aq.
Glycerol +
3%H,B0|
0.0156
0.025 (20*) (Gori, 1913.)
6.1 (20'') (Scbolts. I9ia0
16 (20*)
39.8 (20*)
tf
l^.
temp.)
(Bwoniuid
BarlinettOt
1911O
S(X.UBILITY OF MORPHINB IN SbVBRAL SOLVBNTS AT 2$^,
(Schftcfer, 19x3.)
Gms. Gobs.
Sol»««t. ^i^^^ Solvent. C„HrfJQ|.H.O
per 100 oc
Solvent.
per zoooc
SolvenL
Ethyl Alcohol 0.388
Methyl Alcohol 6 . 66
Chloroform 0.04
Benzene insol.
I Vol. CtH60H+4 Vols. CHCU o . 66
+4V0IS. Celi 0.2'
I Vol. CHaOH +4 Vols. CHCU 4 . 54
+4V0IS. QH« as
Solubility of Morphine in Ethyl Ether at 5.5^
^ (Marcbionnesdii, 1907.)
Solvent.
Washed and Distilled Ether
Gms.Mondiine
per zoo Gms.
Sat. SoL
Solid Phase.
0.049 Ci7Hi»N08.HiO
Ether Purified by Distillation over Na o . 263 "
0.56 CitHwNOs
tt
iC
ti
tt
SCX^UBILITY OF MORPHINE IN AqUEOUS SOLUTIONS OF SaLTS AND BaSBS AT
Room Temperature, Shaken Eight Days.
(Dieterkh, 1890.)
In N/io Salt
. or Base.
In N/i Salt
or Base.
|. Salt or B«M.
Grams per
Liter.
Grams per
liter.
Salt or Base.
Mon^iine.
Salt or Base.
Morphine.^
NH«OH
3SI
0.20
3508
0.505
(NH^,CO,
4.80
0.031
48.03
0.040
KOH
4.62
2.78
46.16
...
K,CO,
6.92
020
69.15
0 379
KHCO,
10.02
0.024
100.16
0.040
NaOH
4.00
3 33
40.05
• • •
Na,CO,
S-30
0.09
S3 03
0.14
NaHCO,
8.41
0.032
84.06
0.044
Ca(OH), (sat)
1 .00 (25°)
• • •
• • •
mobphdh 44a
MOBPHIHI AOETATI CH,C00H.C„H,J^0,.3H,0, Morohinc
Hydrochloride HCLC,rH,^0,.3H,0, Morphine Sulphate H^SO*.
(Ci7H,»NOa)a.5HaO, and Apo Morphine Hydrochloride HCLCti
H„NO,.
Solubility in Several Solvents.
(U. s. p.)
Grams per 100 Grams of SolTent.
SolfcoL Acetate. Hydrodiloride. SuliAatc. Apo M. Hyyfaocfaloride.
af. 8cf. "If. ' ST ai*. 8o«. as*. iST*
Water 44.9 50.0 5.81 900.0 6.53 166.6 3.53 ' 6.35
Alcohol 4.6 40.0* 3.4 3.8* 0.33 0.53* 3.63 3.33
Chlorofonn o. 31 ... ... ... ... ... o. 026
£ther ... ... ... ... ... ... o. 053 • • •
Glycerine 19.3 ... so.of ...
♦ 6o». t I5.S*.
100 gma, HiO dissolve 1.69 gms. apo morphine hydrocloride at I5.5^ and 3.04
gins, at 25**.
100 gms. 90% alcohol dissolve 1.96 gms. apo morphine hydrochloride at about
15.5*- (I>ott. 1906.)
100 gms. H«0 dissolve 4.17 gms. morphine hydrated sulfate .sHtO at 15°.
(Power, i88s )
MOBPHINX SALTS (con.)
SoLUBiLriY IN Water and in 90% Alcohol at Ord. Temp.
(Squire and Cfunes, 1905.)
Gms. Salt per 100 cc. Gms. Salt per zoo oc
Mon.hin.Sdt. ^ ^^ M<Hphin.S.U. fU^. j^^
Moiphine Acetate ... i Diacetyl Morphine (Heroine) o.ii 2.5
" Hydrochloride ... 2 " " HCl 50 9.1
" Sulfate ... 0.143 Ethyl Morphine HCl (Dionin) 14.3 20
" Tartrate 10 0.172
100 gms. 4% HCIO4 solution dissolve 0.44 gm. morphine perchlorate at 15^.
(Hofmann, Roth, HObald and Metder, 19x0.)
Solubility op Morphine Salts in Several Solvents at a5^
(Scbaeffer, 19x3.)
Gms. of Each Salt Separately per 100 cc of Each Solvent.
Solvent.
HjSSS&e. ^Xte!* M^JS^. ^Sg|^ ^HO**
95% Ethyl Alcohol 0.606 0.2 3 9.1 4
85% Ethyl Alcohol 1.2 0.4
80% Ethyl Alcohol 2 o. 77
Methyl Alcohol ... ... 4 11. i 66. 6
Chlorofonn Insol. Insol. 66.6 33.3 0.526
Benzene Insol. Insol. 12.5 Insol. Insol.
I Vol. CtH50H+4 Vols. CHCU 0.18 0.0164 66.6 4.5 5
" +4V0IS. CeHe 0.089 0.0133 25 0.71 1.14
I Vol. CHbOH +4 Vols. CHCls ... 0.22 66.6 20 20
" +4V0IS. QH« 0.253 0.066 25 6.6 8.33
Ethyl MORPHINE Ci7Hi70N(OH)(OC,H»).
100 cc. H2O dissolve 0.208 gm. Ci7Hi70H(OH)(OCiH») at 25*. (Schaeflfcr, xgxa.)
" alcohol " 1.33 gms. " *^
" ether " 66.6 " " "
443 £<^l^yl MORPHDIE
Ethyl MORPHINE H7DBOCHLORIDE Ci7Hi7NO(OH)(OC>Hft).HC1.2HsO
(Dionin) (see also on preceding page).
Solubility in Water and in Alcohol. (SchaefiFer, 1912.)
Gms. Ethyl Moiphine HQ
per 100 cc.
r.
Water.
Alcohol.
IS
8.7
3 -85
2S
"•5
S
40
2S
13. 1
SO . ..
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.
loocc. HiO dissolve iogms.ethylmorphinehydrochlorideatord.temp. (Dott,i9x3.)
MUSTARD on. Allyl Isothiocyanic Ester CS:NC|H<.
Solubility in Sulfur by Synthetic Method. (See Note, p. 16.)
(Alexej<
r.
Bw. z886.)
Gim. Mustard On
per 100' Gm9.
Sulfur Layer.
Mustard Oil Layer.
90
100
10
12
.
72
67
110
IS
62
120
124 (crit. temp.)
23
3S
SI
Freezing-point data for allyl isothiocyanate + aniline are given by Kumalcov
and Solovev (191 6). Results for methyl isothiocyanate -h phenanthrene and
methyl isothiocyanate -f naphthalene are given by Kurnakov and Efrenov
(1912).
MYRISTIC ACID Ci,H»COOH.
Solubility in Alcohols. (Ximofeiew, 1894)
Gms. Gfns.
Sat. Sol. Sat. Sd.
Methyl Alcohol o 2.81 Propyl Alcohol o 5.6
" " 21 21.2 " " 21 31.2
31. S 592 " " 36. S 553
Ethyl Alcohol o 7.14 Isobutyl Alcohol o 6.4
" 21 31 " " 21 28
Freezing-point data for myristic acid -f palmitic acid are given by Heintz (1854).
NAPHTHALENE CioHs.
1000 cc. HjO dissolve 0.019 gm. CioHs at o** and 0.03& gm. at 25**. ' (Hilpcrt, 1916.)
Solubility in Acetic and Other Acids. (Timofeiew, 1894)
Add. t*.
Acetic Acid 6.75
21.5
42.5
Si-3
60
Butyric Acid 6 . 75
U It
It tt
tl ((
ti tt
21.5
60
Gms. CioHs per
AriH
i"
Gms.CiaH8per
zoo Gms. Add.
ACIQ.
m •
100 Gms.' Acid.
6.8
Isobutyric Acid
6.7s
12.3
131
Propionic Acid
6 -75
13 -9
311
it tt
21S
23.4
535
tt tt
SO
79.8
III
Valeric Acid
6-7S
95
13-6
ti tt •
21S
17.7
22.1
tt tt
6S
167.4
131-6
nipbthalinb 444
Solubility of Naphthalbnb in Aqueous Ammonia.
(HDpeit, 191&)
SolvcnL
Aq. 5% NH,
Aq. 10% NHa
Aq. 25% NHa
100% NH«
Aq. 2% Pyridine
Solubility in Methyl, Ethyl, and Propyl Alcohols.
(Speyen— Am. J. Sd. [4] X4f 394* 'oa ; at 19.^, de Bniyn— Z. phyak.Chem. 10, 7&|, '99 ; at xz*. Tinib
faew — Compt.rend. xia, 1x37, '91.)
The original results were calculated to a common basis, plotted on
cross-section paper, and the following table read from the curves.
Gms. C^k
per
eot
at:
o\
as-- '
0.030
0.044
0.042
0.074
0.064
0.162
33
120
0.08a
0.24S
In Methyl Alrnhol.
In Ethyl Alcohol.
In Pro
Wt. of X cc.
' SolutioD.
ipyl Alcohol.
t»-
Wt. ol 1 cc
Sohidon.
Gms. CioHs
per xoo Gms.
CHtOH.
Wt. of X cc.
Solution.
Gms. CtiJEIa
per xoo Gms
CsHsOH.
Gms-CtA
per zoo Gms.
CsHtOH.
0
0.8194
348
0.8175
50
0.8285
4. 45
10
0.812
5.6
0.814
7.0
0.824
5-6
20
0.807
8.2
0.810
9.8
0.821
8.2
25
0.80s
9.6
0.809
"•3
0.820
9.6
30
0.804
II. 2
0.809
13 -4
0.820
II. 4
40
0.805
16.2
0.812
19-5
0.823
16.4
50
0.813
26.0
0.822
35 0
0.837
26.0
60
0.837
50.0
0.855
67.0
0.867
50.0
65
0.870
« • «
0.890
96.0
0.897
80.0
70
0.9023
(68<^) . . .
0.930
179.0
0-933
134. 1 (68.5^
Equilibrium in the System Naphthalene, Acetone, Water.
(Cady, X898.)
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 method 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
THALBNE
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 xoo Gms. Solution.
f.
Acetone.
Water.
Naphthalene.
6SS
10
89.92
0.08
S3 -3
19.91
80
0.09
4S
29.92
69.67
0.41
38
40.81
S8.22
0.97
32.2
48.67
48.68
2.6s
28.5
57.43
36.64
5-93
28.2
60.43
25 -75
13 82
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.
(BQdmer, 1905-06.) (Synthetic Method used.)
Crit. Temp.
Cms. CmHs per
100 Gma. Sat. Sol
34-8
8
64
54
80
100
100 gms. 95% formic acid dissolve 0.30 gm. naphthalene at 18.5^ (Aschan, 1913 J
loogms. 95% formicacid dissolve 3.44 gms. a nitronaphthaleneat 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 op Naphthalenb in:
Carbon Tetra Carbon Dl
Chloride, Sulphide.
(ScfarSder — Z. phvsflE. (Arctowaki — CompL
Ch. II, 457i *93') teuLiai, lajf'os; Eurd.)
Chloroform.
(Speyera; Etard.)
t».
Wt. of I cc.
Sdutioo.
-108
• • •
- 82
• m •
- so
• • •
- 30
• • •
— 10
• t •
0
1-393
+ 10
I -355
20
1.300
25
1.280
30
I- 25s
40
1. 20s
50
I. ISO
60
1. 090
70
1.040
Cms. CioHg por Gms. CioHa pet Gms.Cu
100 Grama
too Gms. Sat
&00 Gms. a
CHa«.
Solution.
Solutioa.
. . •
...
0.6a
...
• • •
1.38
...
• • •
2-3
8.8
• . *
6.6
IS -6
• . •
141
19 S
90
19.9
25 S
140
27 s
31-8
20.0
36.3
35 S
23. 0
41.0
40.1
26.5
46.0
49 S
35 S
57-2
60.3
47 S
67.6
73 •»
62.5
79.2
87.3
80.0
903
Note. — Speyers* results upon the solubility of C,oH, in CHCl,,
when calculated to grams per 100 grams of solvent, agree quite well
with Etard's (Ann. chim. phys. [712 S7^» *94 figures, reported on the
basis of grams CioH. per 100 grams saturated solution.
NAPHTH4LINB
446
SOLUBILITT OF NAPHTHALENE IN:
(Schroder; Etard; Speyen.)
Bei
nzene. C
Gms. CjA
per xooGms.
.hlor Benzene.
Gms. C»H|
per 100 Gms.
Hexane.
Gms. CmHi
per 100 Gms.
Tolu
ene.
f.
Wt. of X cc.
Solution.
Gms. CwH|
per xooGms.
Solution.
SdutioB.
Solution.
CA.CH|.
-SO
• • •
...
0.3
• • •
• • •
— ao
• <
1 •
• . •
1.9
• • •
• • •
o
• 1
1 •
. . •
5-5
0.9124
• • •
+ib
27.
5
24.0
9.0
0.9126
15.0
20
36
,0
31.0
14.0
0.913s
28.0
25
40.
5
35 0
175
O.9ISS
36.0
30
45 ■
5
39 0
21.0
0.9180
42.0
40
54.
,0
48.0
30.8
0.9250
56.0
so
65
0
57-5
43-7
0.9350
69.5
60
77
5
705
60.6
0.947s
83.0
70
88.
0
85.0
78.8
0.9640
97-5
80
• 1
> •
• • •
• • •
0.9770
XII.O
Freezing-point data (solubility, see footnote, p. i) are given for mixtures of
naphthalene and each of the following compounds:
a Naphthol. (Crompton 9l Whttely, 1895; KQster,
'95 ; Vignoo, '91 ; Miers ft Isaac, 'oSa.)
fi Naphthol. (Crompton & Whitely, 1895; Vignon,
1891; Isaac, 1908.)
a Naphthylamine. (Vignon, 1891.)
Dihydronaphthalene. (KOster. 1891.)
Nitronaphthalene. (Palasxo & Battelli, 1883.)
Palmitic Acetic Ester. (Batelli & Martinetti, '85.)
Paraffin. (Palazzo & Battelli, 1883.)
Phenanthrene. (Vignon. 1891; Miolati, 1897.)
Phenol. (Yamamoto, '08; Hatcher 9l Skirrow, '17.)
0 Nitrophenol. (Sapoachinikow, '04 ; Kremann, '04.)
p Nitrophenol. (Kremann, 1904.)
2.4 Dinitrophenol. { (Saposchinikow, 1904;
Picric Acid. ( Kremann, 1904.)
Pyridine. (Hatcher & Skirrow, 19x7.)
Pyrocatechol. (Kremann & Janetzky, x9za.)
Resorcinol. (Vignon, x89x; Kremann &
Janetzky, 19x2.)
Stearic Add. (C^ourtonne, 1882.)
Sulfur. (Bylert, .)
Nitrotoluene. (Kremann, 1904.)
1 .2 .4 Dinitrotoluene. "
1 .2 .6 " (Kremann & Rodinis, 1906.)
1.3-4
II
1.3.5
Trinitrotoluene.
pToluidine.
Thymol.
(Kremann, 1904.)
(Vignon, x89z.)
(Roloff, Z895.)
F.-pt. data are also given for the following mixtures:
Nitronaphthalene + Paraffin. (Campetti & Delgrosso, 19x3; Palazao & Batelli, Z883O
a Nitronaphthalene + Urethan. (Mascarelli, 1908.)
a Nitronaphthalene + a Naphthylamine. (Tsakalotos, 19x2.)
P NAPHTHAU5NB SULFONIC ACID C10H7SO.H.
Solubility in Aqueous Hydrochloric Acid at 30*.
(Masson, 19x2.)
dyof Sat.
Solution.
Mols. per Liter Sat. Sol.
Gms. per
Liter Sat. Sol.
A.
HCL QoHtSOiH.
HCI.
CioHySQiH.
1.1925
0 3263
0
679
I • 1653
I. 291 2.470
47.08
514
I. 1553
1.826 2. 117
66.59
440.6
I.III5
4.017 0.762
146.5
158.6
I.II97
7.232 0.089
263.7
18.5
1.1569
0.88 0.063
360.3
I3-I
447 NAPHTHOIC ACID
p NAPHTHOIC ACm C10H7COOH.
One liter of aqueous solution contains 0.058 gm. C10H7COOH at 25^.
Dihydro p NAPHTHOIC ACIDS CioHtCOOH (iiS"* and 161" isomers).
SOLUBILITT OF EaCH ISOMER. DBTBRMINED SEPARATELY, IN WaTBK.
(Dericz and Kamm, 1916.)
oc 0.0Z II Ba(OH)i Solution Requued
«• per 10 oc of the Sat. Solutionis the:
•^. A
1x8" Isomer.
i6z* Isomer.
0
0-39
0.19
20
0.56
0.34
40
1-34
0.69
55-56
2.89
I -45
71-72
6.7
3.48
80
9-3
4.68
90
14.6
8
96-97
20.1
10. s
f NAPHTHOL ChHiOH.
Solubility in Water.
Gnis.^CttH,OH
f.
per zoo cc
Sat.SoL
Aathoritj*
"•5
0.044
(Kuriloff, 1897.)
25.1
0.074
(KOater, 1895.)
29.S
0.0876
(Kiiriloff, 1898.)
Data for the solubility of isomorphous mixtures of fi naphthol and naphthalene
in water at 25.1® are given by Kilster (1895).
Solubility of jS Naphthol in Aqueous Solutions of Picric Acid at 29^
(Kuiiloff. 1898.)
Mob. X 10^ per zoo cc Sdutioa.
Cms. per zoo cc
. Solution.
CiH|.0H(N0i)|.
CioHtOH.
CeH/)H(NQi>,.
C10H7OH.
Sotid Phase.
0
609
0
0.0877
^ Naphthol
S4
61S
0.0124
0.0886
II
68. s
620
0.0157
0.0894
" -^ Naphtholpknte
69
607
0.0158
0.087s
^ Naphtholpicrate
69
597
0.0158
0.0860
u
88
494
0.0212
0.0712
«
100
390
0.0229
0.0562
II
196
180
0.0449
.0.0259
M
308
los
0.0706
O.OI51
M
933
8
0.2138
O.OOII
" +PicricAcid
928
0
0.2126
0
Picric Arid
Data are also given for the distribution of fi naphthol between water and ben-
zene. The mean of the cone, in CeH* layer divided by cone, in HsO layer is given
as 67. ^ The temperature is not eiven. The determination of the fi naphthol was
made by an iodine titration method.
The coefficient of distribution of fi naphthol between H|0 and CHCU at 25^ is;
cone, in HsO -f- cone, in CHCls — O.0171. (Harden. Z9Z4.)
Data for the solubility of fi naphthol, picric acid (naphthol picrate) and their
mixtures in benzene, determined by the synthetic (sealed tube) method, are given
by Kurilof! (1897a).
100 cc. 90% alcohol dissolve about 55 gms. /9 C10H7OH at 15.5^.
(Greenish and Smith, Z903.)
100 gms. 95% formic add dissolve 3. 11 gms. fi CioHrOH at 18.6**. (Aschan. 1913)
P NAPHTHOL 448
Solidification Temperatures of Mixtures of fi Naphthol and Salol.
(Bellucd, 19x2.)
t*of Gms. d CioHjOH per t^of Gms. A CuHjOH per
Solidificatkm. xoo Gms. Mixture. Solidificatioa. zoo Gms. Mixture.
121. 7 ICO 80 40
1x6. 5 90 68 30
III 80 525 20 .
105 70 34 Eutec. 10
975 60 38.5 s
88 50 42 o
Freezing-point Data (Solubility, see footnote, p. i) are given for the
Following Mixtures:
a Naphthol -f a Naphthylamine. (Vignoo, 1891.)
II ^^ 11
" 4- Dimethylpyrone. (Kendall, 1914)
" 4- Resorcinol. (Vignon, 1891.)
" 4- P Toluidine. (Vignon, 1891; Philip, 1903.)
0 Naphthol + a Naphthol. (Vignon, 1891; Crompton and White^y, 2895.)
4- a Naphthylamine (Vignon, 1891.)
II
" + Dimethylpyrone (Kendall, 1914.)
" 4- Picric Acid. (Kendall, 1916.)
" 4- Sulfonal (Bianchini, 19x4*)
<i -^
-f p Toluidine. (Vignon, 1891.)
a NAPHTHTLAMINE p Sulfonic Add, 1.4 a CioHeNHs.SOiH.
a NAPHTHYLAMINE 0 Sulfonic Add, 1.2 a CioH«NHs.SOiH.
Solubility of Each Separately in Water.
(Dolinski, 190^ "*
Gmi. per xoo Gms. HflO. Gms. per 100 Gms. H/).
V • p Sulphonic c Sulphooic ^ • p Sulphooic o Sulphooic
Ac. Ac. Ac. Ac.
o 0.027 0.24 50 0.059 0.81
10 0.029 0.32 60 0.075 I -OX
20 0.031 041 70 0.097 1.37
30 0.037 0.52 80 0.130 1.80
40 0-048 0.65 90 0.175 2.40
100 0.228 3.19
The coefficient of distribution of fi naphthylamine between benzene and watei
at 25^ is; cone, in CeHa-r- cone, in HsO — 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 4- Phenol.
(PhiKp, 1903.)
+ Quinol.
(Philip & Smith, 1905.)
" 4- Resorcinol.
( " ; Vignon. 1891.)
-f ^ Toluidine.
fi Naphthylamine 4- rhenol.
(Vignon, 189X.)
(Kremaim, X906.)
" 4- Rescorcinol.
(Vignon, 189X.)
+ /> Toluidine.
tf
P NAPHTHTL BENZOATB CsHtCOOCioH,.
100 gms. 95% formic acid dissolve 0.25 gm. QHtCOOCioH? at i8.6*.
(Aschan, X913.)
NAJEtCEINE C»H,7N08 + 3HsO.
100 gms. HsO dissolve 0.078 gm.'narceine at 13''; 100 gms. 80% alcohol dissolve
0.105 gm. at I3^
100 gms. CCI4 dissolve o.oii gm. narceine at 17^ (Schinddmeiser, 1901); 0.002
gm. at 20® (Gori, 191 3).
449
NABCOTINE CioHaNa.
Solubility in Several Solvents.
NABCOTINE
Solvent.
V.
\»ms. xNarcoune per
100 Gms. Solvent.
Authority.
Water
IS
0 I*
(Guerin, 19x3.)
Water
20
0.0044S
(ZaUi, 1910.)
Acetone
IS
41.96*
(Guerin, xgxj-)
Aq. so Vol. % Acetone
IS
0.7*
u
Aniline
20
2S
(ScholU, X9X2.)
Pyridine
20
2.3
tt
Piperidine
20
1-7
K
Diethylamine
20
0.4
II
Carbon Tetrachloride
20
1.04
(Gori, 19x3.)
Trichlor Ethylene
IS
6.S
(Wester and Bruios, 1914.)
Oil of Sesame
20
0.086
(Zalsi, X9xa)
NEODYMIUM
r.
rfy of
Sat. SoL
Cms. NdCU.6H<!0 per too Gms.
Sat. SoL
71.12
Water.
246.2
* Per zoo oc. solvent.
CHLORIDE NdC1.6H^.
Solubility in Water. (Matignon, 1906, 19090
Method of obtaining saturation not stated.
Gms. NdCUpcr 100 Gms.
Sat. SoL Water.
13 1-74 4967 98.68
100 ... ... 140 ... • • .
100 gms. abs. alcohol dissolve 44.5 gms. (anhydrous) NdCli at 20**. Saturation
was obtained by spontaneous evaporation of the solution over H2SO4.
(Matignon, 1906.)
100 gms. anhydrous pyridine dissolve 1.8 gms. anhydrous NdCU at about 15®.
Saturation obtained by daily agitation of the solution for some weeks. (Matignon, '06.)
NEODYMIUM COBALTICYANIDE Nd,(CoC6Ne),.9H20.
1000 gms. aq. I o%HCl((fi6~ 1.05) dissolve 4. 19 gms. salt at 25^ (James &Wil]and/x6.)
NEODYMIUM GLYCOLATE Nd(CsH,0«),.
One liter HsO dissolves 4.609 gms. salt at 20**. (Jantsch & GrOnkraut. I9X2-X3-)
NEODYMIUM MOLYBDATE NdsCMoOOs.
One liter HaO 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. HNOj of dj^^ i.325(= 51.59 Gms. HNOj per
100 CC-) AT l6^ (Jantsch, x9ia.)
Gms. Hydrated
Double Salt per
100 Gms. Sat. SoL
97.7
116. 6
iSi-6
177
296
Double Salt.
Formula.
Neodymium Magnesium Nitrate [Nd(N08)6]2Mg8.24H20
Nickel
Cobalt
Zinc
Manganese
NEODYMIUM OXALATE
«
it
(t
H
(t
ti
u
Ni,
(t
CO,
a
Zn,
it
Mn,
it
ti
it
NdjCCOOi.ioHsO.
Solubility in Water at 25® by Electrolytic Determination.
(RimlAch and Schubert, X909.)
One liter sat. solution contains 0.0053 i^S^* equivalents of anhydrous salt « 0.49
milligram.
SouuBiLiTY IN Aqueous ao% Solutions of Methyl, Ethyl and Triethyl
Amine Oxalatbs, Roughly Determined, ((jrant and James, X9X7O
100 CO. aq. 20% methyl amine oxalate dissolve 0.027 gm. neodymium oxalate.
etJiyl ' aio7
triethyl " li " 0.065
it
tt
It
II
II
II
11
44
NEODYMIUM OXALATE
450
Solubility of Neodymium Oxalate in Aqueous Solutions of
NeoDYMIUM Nitrate at 25^. Junes and Robinson. 19x3.)
(The mixtures were constantly agitated at constant temperature for twelve
weeks.)
Gnis. per TOO Cms. Sat. SoL Cms. per xoo Gms. Sat. Sol.
Nd,(COJ,.
Nd.(NQ,)e.
Solid Phase.
Nd,(Q04),.
■' ^
NdiCNOi)..
Solid Pbue.
0.18
6.46
Nd,(Q04)sXiH,0
2.07
47 64
Nd.(CVO.)..iiH«0
O.S4
12.23,
«
2-54
SO
52
M
0.76
17.78
u
2.89
S2.
82
It
0.8s
22.67
u
3-1?
54
.67
M
0.96
27 -43
tt
2.21
S6
48 probably
I.aJ.24
1.28
31 36
u
1.44
59
68
Nd,(NQ,),(?H/))
1.38
35-26
u
1-33
59
67
II
1.66
38.70
If
1. 21
59
.70
II
1.88
42.13
u
0.96
59
75
«
1.96
44.82
t$
» • •
60
46
fi
1 .2i.24> Nd,(C04)i.2}Nd,(NO.)«.24H20.
NEODYMIUM Dimethyl PHOSPHATE NdsKCH^sPOJe.
100 gms. H2O dissolve 56.1 gms. Ndi[(CHi)iP04l« at 25** and about 22.3 gms.
£tt 95 ■ (Morgan and James, 19x4.)
NEODYMIUM SULFATE NdsCSOOi.
Solubility in Water. .
(Muthmann and Rolig, 1898.)
f.
O
16
30
Gms. Ndt(S04)3 per 100 Gms.
/ • N
Solution.
8.7
6.6
4-7
Water.
9-5
7-1
5
r.
SO
80
108
Gms. NdsCSOf)! per 100 Gms.
jk
Solution.
35
2.6
2.2
Water.
3.7
2.7
2.3
NEODYMIUM SULFONATES.
Solubility in Water.
Sulfonate.
Formula.
Gms. Anhy-
M drous Salt per
100 Gms.
HtO.
Authority.
Neodymium:
m iNitrobenzene NdlCH4(NOj)SOila.6HjO 15 46.1 (Holmbeijf, 1907.)
Bromo { Sulfonate Nd[C6H,Br(i)NO,(4)SQ,(3)lt.8H,0 25 7 . 25 (Kats & James, 19x3.)
NEODYMIUM TUNGSTATE Nd^OVO^i.
One liter HiO dissolves 0.0190 gm. Nd2(W04)« at 22®, 0.0168 gm. at 65® and
0.0152 gm. at 98''. The mixtures were not constantly agitated and only two
hours were allowed for saturation. ' (mtchoock, 1895.)
NEON Ne.
Solubility in Water.
(v. Antropoff, X9o9'-xo.)
t". o. xo. 20. 30. 40. 50.
Coef. of Absorption /3 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 HsO
for volume of HiO in the formula Absorp. coef. Kuenen =» — ^ — rrr-F^rm*
massofHiOXP
NEUBINE FEBCHLORATE CH..CH.N(CH,)30H.HC104.
100 gma. HiO dissolve 4.89 gms. of the salt at 14.5° (Hoimann & HfiboU, tgjf.)
451
NICKEL BBOMATB
NICKEL BBOMATB Ni(BrQ,)t.6H«0.
100 gms. cold water dissolve 27.6 gms. nickel bromate.
NICKEL
BL BB
OBflDE NiBrt.6HA
Solubility
IN Watbk.
(^:tud. X894.)
GmkNiBrt
Gms-NiBf^
Gm9.NiBih
«•.
per zoo Gms.
f.
per zoo Gms.
f.
per zoo Gms.
Solution.
SolutMO.
SolutKMk.
— 20
47-7
2S
57-3
80
60.6
— 10
SOS
30
58
100
60.8
0
S3
40
591
120
60.9
+10
ss
SO
60
140
61
20
S6.7
60
60.4
NICKEL CABBONATB NiCQi.
One liter H«0 dissolves 7.789] X lO"^ mok. NiCQi » 0.0925 sm. at 25^
(Ageno awTVa]]*, 1911.)
NICKEL CABBOZTL.
100 gms. of the aqueous solution saturated at 9.8^ contain 2.36 cc. of the vapor
» 643 milligrams Ni. In blood serum it is 2} times as soluble. (Armit, 1907.)
HIOKBL OHLOBATE Ni(aO,),.
*
Solubility in Water.
(Meuaaer — Bcr. 3S» Z4X9, '09.)
Gms.
Mob.
Ni(aQi)9
periooums. per 100
Sohitiao. Mols.^.
oGm
SoUd
Phase.
Gms. Mob.
Ni(aot)t Ni(ao«yt
per 100 Gms.
Solutka
xoo
i.HaO.
sooa
Phase.
-18
- 8
O
+ 18
40
49-55 7*84 Ni(aOs)sj6HaO
51.52 8.49
52.66 8.88
56.74 10.47
64.47 15-35
48
55
65
79
-13
- 9
5
5
67
68
69
75
31
26
60
78
05
50
85
62
16.65 Ni(aO|)s^HiO
1759
18.01
24.68
3-73 ^
2-90
8p. Gr. of solution saturated at + 18 — 1.661.
According to Carlson (1910) 100 gms. sat. sol. in HiO at 16^ contain 64.1' gms.
Ni(C10t)i and dit of sat. sol. » 1.76.
NICKEL PerCHLORATB Ni(C10«)t.9H^.
Solubility in Water.
(Goldblum and Terlikowaki, X9Z2.)
Gms.
Gnu.
f.
dci
Ni(a04)t
periooGms.
HtO.
Solid Phase.
f.
tfof
Sat. Sol. 1
^"i^t SoKd Phase.
H,0.
0
m
0
ke
-21.3
• • •
92.5rNi(CK)|),.9H^
— 10.9
33 19
tt
0
1-573
104.6 Ni(CI04)..5Bd0
— 21.3
46.68
u
7.5
I 576
106.8 Ni(aQ«)«.sHdO
"30.7
70
tt
18
1-576
no. I **
"49
... Ice + Ni(C304)a.9H/)
26
1.584
112. 2 "
-30.7
90
^(ao4),.9GV>
45
I -594
118. 6
NICKEL GHLORIDI
AS2
NICKIL GHLORIDI
NiCl,.6H,0.
S(x.UBiLiTY IN Water.
(Etard, 1894.)
f.
-17
o
+10
20
Gms. NiClt
per looGms.
Solutku.
29.7
35
37-3
391
Gnu. NiCIa
4*. per 100 Gms.
Solution.
as 40
30 40.8
40 42.3
SO 43-9
NiCI,
f*. per 100 Gm.
SolutioD.
60 45. I
70 46
78 46.6
icx> 46.7
(Ditte, 1881.)
1000 cc. sat. HCl solution dissolve 4 gms. NiCU at I2^
100 gms. abs. alcohol dissolve 10.05 gms. NiCU at room temperature.
100 gms. abs. alcohol dissolve 53.71 gms. NiCls.6HtO at room temperature.
(&fidtker, 1897.)
100 gms. abs. alcohol dissolve 2.16 gms. NiClt.7H«0 at 17^ and 1.4 cms. at 3^
(de firuyn, 1893.)
100 gms. saturated solution in -glycol contain 16.2 gms. NiCU at room tem-
perature, (de Coninck. 1905.)
^ 100 CC. anhydrous hydrazine dissolve 8 gms.' NiCls at room temp, and solu-
tion is colored violet. (Welsh and Brodenon, 19x5.)
100 gms. 95% formic acid dissolve 5.9 gms. NiCls at 20.5^. (Aachan, 1913.)
When I gm. of nickel, as chloride, is dissolved in 100 cc. of 10% aq. HCl and
shaken with 100 cc. of ether, o.oi per cent of the Nickel enters the ethereal layer.
(Mylius, 191 !•)
MICKIL CITRATB Ni,[(C00CH,)sC(0H)C00],.2H«0.
'100 cc. sat. solution in water contain 0.28 gm. Ni —[0.94 gm. anhydrous
salt at 10'
(Pkkering, 1915.)
MICKIL Potassium CITRATE K4Ni[(COOCH0>COHCOO]t.
100 cc. sat. sol. in water contain 3.9 gms. Ni « 41 gms. salt at lo^
(Pkkcring, 1915.)
NICKEL HYDROXIDE Ni(OH)i.
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 NH| the gms. Ni per liter
varied from 0.17 to 0.83. For 4 n NH<, the gms. Ni per liter varied from 0.36
to 1.8. (Bonsdorff, 1904.)
NIOKBL lODATE
Ni(IO.)..
Solubility
IN
Water.
(Meuner — Bcr
,34f 2440. 'oi.)
Gms.
Mols.
Gms.
Mob.
to NidCM,
* per 100 Gms.
Ni(IOJ| SoUd
perxooMols. Phase.
t».
Ni(IO»>,
per 100 Gms.
Ni(I08)s
per 100 Moll
Solid
1. Phase.
Soludoa.
H,0.
Solutioa.
HaO.
0 0.73
0033
NiaO»),-4H,0
18
o-SS
0.0245
NiaO^^HflO (a)
18 I .01
0.04S
u
SO
0.81
003s
M
30 I. 41
0.063
*t
75
1.03
0045
M
0 0.53
0.023
NiaOfe)3.aHsO (x)
80
1. 12
0.049
W
18 0.68
0.030
14
30
I 135
0.050
Mao*),
30 0.86
0039
«
SO
1.07
0.046
M
50 1.78
0.080
««
7S
1.02
0045
M
8 0.52
0.023
NiaO,)j.aH,0 (a)
90
0.988
0.044
M
(I)
aDihydmte.
(a) /I Dihydrate.
453
NICKEL IODIDE NiIs.6HaO.
Solubility in Water. (Etaxd. 1894O
NICKEL IODIDE
f.
Gms. Nilfper
t*
Gms. Nil| per
1*
Gnu. Nil. per
looGm*. Sohitioa.
xoo Gms. Solutk»
w •
xoo Gms. Soltttkm.
w •
—20
Sa
25
60.7
60
64.8
0
55-4
30
61.7
70
65
10
S7-S
40
63.5
80
65.3
20
S9-7
so
64-7.
90
65-3
By interpolation the tr. pt. for NiIs.6HsO + NiIt.4H«0 is at 43*.
NICKEL MALATE Ni[CHiCH0H(COO)h.3HA
100 cc. sat. solution in water contain 0.02 gm. Ni » 0.06 gm. salt at lo^
(Pickering, 19x5.)
NICKEL NITBATE Ni(NO,)a.
Solubility in Water.
Gms.
Mds.
v««aip» r ~ini ■ ^m »• j
Gms.
WW./
Mob.
^. Ni(NO»)a
* * per xoo Gms.
Ni(NO|)s
per xoo Mo
Solid
ft*
Ni(NO|>9
Ni(NC^
periooMols
Solid
Is. Phase.
V .
per xoo Gms.
Phase.
Solution.
HsO.
SoludoQ.
HsO.
-2J 39.02
6.31
Ni(NOk)a^H|0
20
49.06
9.49
Ni(NOk)a^^
-21 39.48
6.43
M
41
55"
12. 1
(4
-lo-s 4413
7-79
«4
S6-
7 62.76
16.7
(•
-21 39.94
6-55
Ni(NOfe)s.6HsO
58
61.61
15 -9
Ni(NO|)s.3HflO
-12.5 4159
7.01
u
60
61.99
16.0
•«
— 10 42.11
7.16
H
64
62.76
16.6
••
— 6 43.00
7-44
•4
70
63 -95
17.6
u
0 4432
7.86
M
90
70.16
23 I
M
+ 18 48.59
9-3
•»
95
77.12
33-3
(«
100 gms. sat. solution in glycol contain 7.5 gms. Ni(NOi)t at room temperature.
(de Coninck.)
100 CC. anhydrous hydrazine dissolve 3 gms. Ni(NOi)t at room temp.
(Welsh aod Brodenon, 19x5.)
NICKEL OXALATE Ni(COO)s.
100 gms. 95% formic acid dissolve o.oi gm. at 19.8^ (Asdum, 19x3.)
NICKEL SULFATE NiS04.7HsO.
Solubility in Water. (Steele and Johnson, X904; see also Tobler. Etard and Mulder.)
t:
Grams NiSO< per
100 Gnu.
Solid
Phase.
t».
Grams NiS04 per
100 Gms.
SoUd
Phase.
Solution.
Water.
Solution.
Water.'
-5
20.47
25-74
NiSO«.7H|0
33-0
30.25
43-35
NiS04j6HsO
0
21.40
27.22
"•
35-6
30.45
43-79
« (bhie)
9
23-99
31-55
«
44.7
32.45
48.05
41
33.6
27.48
37-90
M
50.0
33.39
50.15
14
30
29.99
42.46
M
53 0
34.38
52.34
11
32 -3
30.57
44.02
14
54-5
34-43
52.50
NiS04j6HsO
33
31-38
45-74
14
57-0
34.81
53-40
" (gncD)
34
31-29
45-5
M
60
35-43
54.80
M
32 -3
30.3s
43-57
NiSO«^HsO
70
37 29
59-44
M
33 0
30.25
43-35
•• (blue)
80
38.71
63.17
M
34 0
30.49
43-83
«
99
43-42
76.71
M
Transition points, hepta hydrate 4=t hexa hydrate ~ 31*5*
Heza hydrate (blue) ^ hexa hydrate (green) «- 53.3 .
NICKIL 8ULFATK
4M
Solubility op Mixturbs op Nickbl Sulphatb and Coppbr Sulphatb.
(Pock— Z. Kntf. MiA. aM, 387. '970
Results at 35^.
Cms. per xoo Gms. HjO*
Mol. per cent in Sohitka.
Mol. per cent in Solid Phaae.
Cryrtal
CaSO«. NiSO«/
'C11SO4.
NiSO«.
CUSO4.
NiSOi.
Fonn*
9.6a 583.9
1-57
98-43
0.35
99-65
Shombk
41.66 484.4
7-69
92.31
2.12
97.88
i«
75-39 SS3-S
11.66
88.34
4.77
95-23
Tetngcoal
106.40 506.5
16.92
83.08
6.52
93 48
M
172.0 483.8
25-63
74.37
13.88
86.17
M
186.9 468.0
27.90
72.10
(18.77
(94.91
81.23
5 09
TetncQoal
•nidinic
Results at 67®.
20.04 729 -3
2.65
97-35
0.93
99.07
Monocdnlc
66.01 706.2
8.31
91.69
2.86
97.14
u
88.08 501.6
13-55
86.45
3-92
96.08
M
47-94 675.0
16.39
83.61
6.66
93-34
M
249-9 747-8
24.46
75-54
22.32
77. 68
(MaaocUnic
1 Trirlinir
Solubility op Mixtures op Nickel Sulphatb and Sodium Sul-
phate, ETC.
(Koppel; WeUd — Z. phyiik. Chem. 5a, 401, '05.)
Gms.
per xoo
Gms. I
per xoo
Mols. per xoo
t».
Gms. Solution.
Gms. HsO.
Mols.
H,0.
Sofa'rf
Phaae.
NiSO*.
NaaSO«.
'NiSO«.
NasSO«.
NiSO*.
NasSO*. '
0
16.94
7.61
22.46
10.00
2.61
1.28
5
17.99
10.85
25.28
15
24
2.94
1-93
■^,«oio-
10
18.97
1385
28.26
20.
64
329
2.61
20
18.76
17.21
29.31
26.
87
3.410
3 404
NiNai(SO,)i-lHsO
25
17-85
16.54
27-33
25-
33
3. 181
3 208
•t
30
16.74
15-34
24.64
22.
58
2.868
2.861
M
35
16.28
14.91
23.66
21.
67
2.753
2.744
M
40
15-35
14.49
21.88
20.
65
2.546
2.616
M
18.5
19.61
16.49
30 70
25
80
3 56
327 '
20
20.13
16.15
31 59
25
35
3 67
3.21
25
30
21.20
22.60
14.77
12.80
33'^^
34-98
23
19
06
82
3-85
4.07
2.92
2.59
■^'S2»^+
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
372 '
20
15.48
20.18
24.06
31
37
2.80
3-97
■'^^^aa?+
25
10.92
24.12
16.81
37
13
1.96
4.70
30
6.40
28.71
9.87
44
25
I-I5
5-60 J
35
40
4.54
4.63
31-65
31-37
7-13
7-24
49
49
59
03
0.838
0.843
6.28 I
6.21
NIN^JmH^ +
455 NICKIL SULFATE
Solubility of Nickel Potassium Sulfate NiKi(S04)i.6HiO in Water.
(Tobler, 1855; v. Hauer, 1858.)
f.
Gms. NiKt(S04>i per zoo Gms. H^.
(Tobler.) (v. Haner.)
f.
Gms. NiEs(SQ«)t per zoo Gms. H^.
, X .^
(Tobler.) (v. Hauer.)
0
S'S.
SO
30
10
8.9
60
35.4 20.47
20
30
13 -8 9-S3
18 . 6 ...
70
80
42 ....
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
un
[IS. 1:^10^/4 per luu \jUi
IS. osi. 001. lu KAmiaia. ^
wnui
CILOH
insolvent.
o(HjO)
NiS0<.7H|0 u
Solid Phase.
36.4
NiS0..6H^aas
Solid Pblne.
26 (low)
NiS04.6IL0/»as
Solid Phase.
27.2
NiSO^^HiO as
SolidPhaae.
10
19.7
22(?)
20.4
...
20.
30
131
6.8
14.7
6.6
14
7-5
14.8
40
2.8
2.4
31
SO
60
1-3
0.8
I
0.4
1.4
0.6
1-4
70
80
0.6
0.6s
0.2
0.2
0.4
0.4
0.66
8S
i-S
03
0,7
90
9S
100
S-7
II
16.8
1.2
6
12.4 (low)
2.5
9(?)
15.7 (low)
738
NiS04.6HsO a is greenish blue. NiS04.6HsO is more greenish than the a salt.
Solubility of NiSO4.3CH1OH.3HjO in>queous CHiOH at 14**.
(de Bruyn, 1903.)
Wt. Per cent
CH^H.
86
87
88
89
Approximately two hours were allowed for attainment of equilibrium.
In solutions containing more than 15% HiO the salt is gradually transformed
to NiS04.6H,0/3. ti y
100 gms. absolute ethyl alcohol dissolve r.4 gm. NiS04.7HjO at 4** and 2.2
gms. at 17^ (de Bruyn, x89a.)
100 gms. sat. solution in glycol contain 9.7 gms. NiS04 at room temp.
(de Coiunck, 1905.)
NICKEL SULFIDE NiS.
One liter HiO dissolves 39.9 X lo"* gm. mols. NiS = 0.0036 gm. at I8^ by
conductivity method. (Weigd, 1906.)
Fusion-pointdata for NijS+NajS and NUSj+NajS are given by Friedrich (1914).
Gms. NiS04 per
Wt. Per cent
(jms. NiS0« per
xoo Gms. Sat. Sol.
CH«0H.
xoo Gms. Sat. SoL
1-93
90
0.70
1-73
92.5
0.50
1.48
95
0.4S5
I-2S
97.5
0.77
1. 01
100
372
NICOTINE
456
NICOTINE C10H14NS.
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. o
14.8
32.2
49.0
66.8
80.2
82.0
Temperature of
Appearance of
Two Layers.
Degrees C.
94
89
75
6S
61
64
72
87
129
Temperature of
Homogeneity.
Degrees C.
95
200
210
20s
190
170
130
Additional data for the above system are given by Tsakalotos (1909). The
values for the temperatures of saturation are in general, from 1° to 5^ lower than
those of Hudson.
NIOBIUM Potassium FLXTOBIDE NbKiF?.
Solubility in Water and in Aqueous HF and Aqueous KF Solutions.
(Ruff and Schiller, 19x1.)
* The determinations were made in platinum vessels. The mixtures were
shaken for 3 hour i>eriods at constant temperature and the saturated solutions
filtered through platinum funnels.
Gms. per xoo Cms. Sat. Solution.
Solvent.
Water
16
NbF».
A
KF.
2.98
HF.
0.3s
SoUd Phase.
KtNb0Fi.B/)
Aq. 10.95% HF
" 7.41% KF
" 7.39% KF
16
16
16
16
7.07
4.33
1. 16
2.67
S-33
2.32
554
6.04
435
10.43
0.13
S-39
K|NbOF».H^+KtNbFT
KtNbFT
KtNbOF».H^
K«NbOF».H^+K«NbFT
Water
Aq. 4.8i%KF
8S
80
30.39
11.66
14.68
10.08
0-3S
I 53
K«Nb0Fs3^0(?)
M
NTTBIC ACm HNQ,.
Distribution of Nitric Acid between Water and Ether at as'.,
(Bogdan, 1905, 1906.) -- -
Mols. HNQi per Liter of:
Mols. HNQi per Liter of:
HiO Layer.
Ether Layer.
, ..
H,0 Layer.
Ether Layer.
0.914s
O.08SS
0.09005
O.OO181
O.481I
0.0278
0.04749
0.00064
0.2644
0.00894
0.02760
0.00029
0.1392
0.00278
0.02462
0.00025
457
NITBIC ACm
Reciprocal Solubility of Nitric Acid and Water, Determined by the
Freezing-point Method.
(Kllster and Kzemann, 1904; we also Pickering, 1893.)
Gms. HNOi
Gms. HNOk
t*. per xoo Gms
m
Solid Phase.
f.
per xoo Gms.
Solid Phase.
Sat. Sol.
Sat. Sol.
— 10 13.9
Ice
-40
69.7
HN0|.3H«0
— 20 22.9
M
—42 Eutec.
70. s
" +HN0«.H«0
-30 27.8
fl
-40
72.5
HNOb.B^
-40 315
f«
—38 m. pt.
77. 75
II
-43Eutec. 32.7
II
+HNQ|.3H«0
-40
82.4
II
-40 34 I
HN0b.3H«0
-SO
86. s
M
-30 40
M
-60
88.8
II
— 20 49.2
U
—66.3 Eutec.
89.9s
« +HNOb
-i8.sm.pt 53.8
U
-60
91.9
HNOk
-20 58.5
M
-SO
94.8
II
-30 ^5-4
U
—41.2m.pt.
ICO
M
NITBOOIN N,.
Solubility in Water.
OHnnkler-^Ber. 34, 36061 'px; Braun— Z. phyA. Chem. 33, 73ai '00; Bohr and
44* 3x8> '0X-)
Bod:«Wied.Aii»
f
a 01 ADOGrpooi
» p.
-Solnhnity"B'.
0.0233*
ff.
0
0.0235*
o.o239t
■■■t
0 .00239*
s
0.0208
0.0215
00217
0.0206
0.00259
10
0.0186
0 .0196
0.0200
0.0183
0 .00230
IS
o-oi68
0.0179
0.0179
0.0165
0.00208
30
0.0154
00164
0.0162
O.OI5I
0.00189
as
00143
0.0150
0.0143
0.0139
0.00174
30
00134
0.0138
0.0128
O.OOI61
3S
00125
0.0127
00118
0.00148
40
0.0118
O.OII^'
O.OIIO
0.00139
SO
00109
0.0106
0.0096
O.OOI2I
60
0.0102
o.oioo
0.0082
0 00105
80
0.0096
...
00051
0.00069
100
0.0095
0.0100
0.0000
0.00000
• w.
t B. and B.
$B.
For values of ^, fi\ and q, see Ethane, p. 285.
Single determinations of the solubility of nitrc^en in water reported by HQfner
(1906-07), Bohr (1910), MGller (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 fi. Drucker and Moles (1910), {[ive 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 ot nitrogen in water and in sea water is given by
Coste (1017).
Data for the solubility of the nitrogen of air in water are given by Fox (1909a).
The oxygen was removed from air and the solubility of the residual N + i.i8^%
argon was determined. After making correction for the argon, the followmg
formula for the solubility of pure nitrogen in water was deduct:
1000 X coef. of abs. fi = 22.998 — 0.5298 / + 0.009196 fi — 0.00006779 fi.
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.
nTEOOSN 458
S(».UBiLiTY OF Nitrogen in Sea Water.
(Fox, 1909a).
Before using the sample of sea water for the solubility determinations it was
found necessary to add acid, otherwise the COi could not be boiled out or the
precipitation of neutral carbonates prevented. The very small amount of add
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 dr^ atmosphere of 760 mm. pressure.
The calculated fcnrmula expressing the solubility is:
1000 a » i3.6to — 0.4304/ + 0.007453/" — 0.0000549^
— Cf (0.2172 - 0.007187 / + 0.0000952 fi).
f-o-.
4*.
8*.
«•. -
i6*.
ao*.
*••.
a8*.
18.64
17.03
15.63
14.45
13.45
12.59
11.86
11.25
17- 74
16.27
14.98
13.88
12.94
12.15
11.46
10.89
16.90
15.51
14.32
13.30
12.44
11.70
11.07
10.52
16.03
14.75
13.66
12.72
".93
11.25
10.67
10.16
1518
14
13
12.15*
"73
10.81
10.27
9.80
14.31
13.27
12.34
"57
10.92
10.36
9.87
9.44
Farts Chlorine
per xooa
O
4
8
12
16
20
A recalculation of Fox's determinations to parts per million, with correction
for vapor pressure, is published by Whipple and Whipple (191 1).
Solubility of Nitrogen in Aqueous Solutions op Sulfuric Acm
Results at 21^ (Bohr, igzo.) Results at 20^ (Christoff. igo6.)
NonnaUtyoC Absorption Coef. Nonnali^of Absorp. Coef. Percent Ostwald Solubility
Aq. HtSOv ^(Bunsen). Aq. HaS04. ^ (Bunaen). HaSOi. Eq>re88ion W
o 0.0156 24.8 0.0048 o 0.01537
4.9 0.0091 29.6 0.0051 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.
(Biaun.)
Corfficimt of Abaorptum of N in Barium Chloride Solutions of:
r. / • ^
13.83 Per cent ix.92 Per cent. 6.90 Per cent. 3.87 Per cent. 3.33 Per cent.
5 0.0127 0.0137 0.0160 0.0180 0.0183
10 O.OII7 0.0125 0.0147 0.0166 0.0168
15 0.0104 O.OII4 0.0132 0.0148 0.0150
20 0.0092 0.0098 O.OI18 0.0132 0.0135
25 0.0078 0.0086 0.0104 0.0114 O.OII9
Coefficient of Absorption of N in Sodium Chloride Solutions of:
IX. 73 Per cent. 8.14 Per cent. 6.4 Per cent. a.za Per cent. 0.67 Per cent.
5 0.0102 0.0127 0.0138 0.0179 0.0200
10 0.0093 O.OII3 0.0126 0.0164 0.0185
15 0.0081 o.oioi 0.0113 0.0147 0.0164
20 0.0066 0.0087 0.0098 O.OI3I 0.0148
25 0.0047 0.0075 0.0083 O.OII3 0.0130
Solubility of Nitrogen in Alcohcx..
(Bunsen.)
t^. o**. 5*. ^o^ I5^ 2o^ 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
NTTBOOIN
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.
Vol. % H/) in
Vol
. % Alcohol in
Dissolved
Mixture.
Mixture.
N(W.
100
0
0.01634
80
20
0.01536
67
33
O.OI719
0
100 (99.8% Alcohol)
0.1432
Solubility of Nitrogen in Several Solvents at 20* and 25®.
au9t.)
Solvent.
/».
In.
Solvent. In-
Im-
Water
0.01634
0.01705
Toluene 0.1235
0.1186
Aniline
0.03074
0.02992
Chloroform 0. 1348
0.1282
Carbon Disulfide
0.05860
0.05290
Methyl Alcohol 0. 141 5
0.1348
Nitro Benzene
0.06255
0.06082
Ethyl Alcohol (99.8%) 0. 1432
0.1400
Benzene
0.1159
0.III4
Acetone 0.1460
0.1383
Acetic Add
0.1190
O.II72
Amyl Acetate 0. 1542
0.1512
Xylene
0.1217
O.I185
Ethyl Acetate 0.1727
0.1678
Amyl Alcohol
0.1225
0.1208
Isobutyl Acetate 0 . 1 734
0.170Z
Solubility of Nitrogen in Petroleum. Coefficient of Absorphon at
lo"* = 0.135, AT 20® = 0.117.
(Gniewasz and Walfisz* 1887.)
Solubility of Nitrogen in Aqueous Propionic Acid and Urea
Solutions.
(BiBun.)
f.
5
10
IS
20
25
11.22 percent.
0.019s
0.0178
O.OIS9
0.0146
0.0130
Coefficient of Absorption of N in C|H|COOH Solutions of:
A ,
3.82 per cent.
9.54 per cent.
0.0204
0.0182
0.0163
0.0147
0.0134
6.07 per cent.
0.0208
0.0186
0.0164
0.0148
0.0134
4.08 per cent.
0.0210
0.0192
0.0169
0.0154
0.0137
0.0209
O.OI9I
0.0167
0.0155
0.0137
Coefficient of Absorption of N in C0(NH|)t Solutions of:
15.65 per cent.
5 0.0175
10 0.0162
15 0.0150
20 0.0140
25 0.0130
X1.9 per cent.
0.0179
0.0167
0.0149
0.0139
0.0130
9.42 per cent.
0.0190
0.0176
0.0x58
0.0146
0.0133
6.90 per cent. 5.15 per cent. 2.28 per cent.
0.0198
0.0183
0.0165
O.OI51
0.0137
0.0197
0.0182
0.0165
O.OI51
0.0135
0.0199
0.0184
0.0171
o.oiss
0.0139
NITROOEN
460
Solubility of Nitrogen in Aqueous Solutions of Chloral Hydrate at 15*-
Results by Mttller, C (1912-13.)
Results by von Hammel (1915).
Gms.
Gms.
Ca,.CH(pH),
per xoo Gms.
1 d% of Aq. Absorp. Coef .
Sol. ^atis*.
CCl«CH(OH)i Abs. Coef. SolubUity In
per xoo Gms. fi at 15*. (OstwaM).
Aq. Sol.
■
Aq. Sol.
0
I 0.0170
0
0.0170 0.01796
15.8
1.0738 0.0158
15
0.0152 0.0160
28.3
I. 1423 0.01423
26.1
O.OI41 0.0149
37.25
I. 1946 0.01300
37.6
0.0123 0.0130
47
1.253s 0.0127s
48.9
O.OII5 O.OI2I
56.52
1.3225 0.0124s
61.3
O.OII4 0.0120
71.5
1. 441 0.01420
70.9
O.OI3I 0.0138
78.8
1.503 0.01492
79.1
0.0156 0.0165
Solubility of Nitrogen in Aqueous Solutions of Glycerol.
Results of MGller, C. Results of
von Hammel' Results of Drucker
(1912-13). (1915).
and Moles (1910).
Gms.
Gms.
Gms.
(^0H)r
CHOH per
100 Gms.
'"sJi"^"' ^Jlk^- ^^
Sol. ^ at 15 . ,^ GiS
Ab8.Coef.
fi at is'.
100 Gms. ^- (Ostwald).
Aq. Sol.
Aq. Sol.
Aq. Sol.
25
I. 061 0.01266 15.7
0.01400
0 0 0.0156
42.3
I. 108 0.00976 29.9
0.01087
16 1.0392 0.0103
SI. 5
I. 133 0.00759 46.6
0.00840
29.7 1.0744 0.0067
58
I. 151 0.00703 57.6
0.00698
48.9 I. 1263 0.0052
80.25
I. 212 0.00530 67.1
0.00635
74.5 I.193I 0.0025
90
1.240 0.00583 77
0.00527
84.1 I. 2213 0.0024
95
1.249 0.00716 88.5
0.00536
99.25 0.00524
Solubility of Ns in pure isobutyric acid oidu = 0.9481, l» (OstmM) » 0.1651.
(Drudcer and Moles, 19x0.)
Solubility of Ns in aq. 37.5% isobutyric acid of (^ >■ 0.9985, /» (Ostwald)
B 0.0396. (Drucker and Moles, 19x0.)
Solubility of Ni in aq. 37.5% isobutyric acid of (^ = 0.9985, l» (Ostwald)
— 0.0384. - (Drucker and Mdes, 1910.)
Solubility of Nitrogen in Aqueous Solutions of Several Compounds.
s^ (HQiner, X906-07.)
Cone, of Aq. Solution.
Aq. Solution of:
Glucose
((
Normality. Gms. per Liter.
I
0.5
Alanine
Glycocol
Aribinose
Levulose
Erythritol
Urea
Acetamide
(a Aminopiopionic Ad4)
( Aminoacetic AdiD
0.25
180
90
45
89
75
150
180
122
60
59
20.18
20.21
20.2
20.19
20.16
20.21
20.25
20.25
20.18
20.22
Abs. Coef. fi,
O.OI215
0.01380
0.01480
O.OI213
O.OI2I2
0.01203
O.OI22I
O.OI32I
0.01477
0.01475
Solubility of Nitrogen in Aqueous Solutions op Cane Sugar at I5^
KMOller, C, X9X2>X3.)
Gms.CifEL0u
per xoo Gms.
Aq. Solution.
11.38
20
29.93
iuof
Aq. Sol.
1.050
1.082
1. 128
Abs. Coef. fi
at IS*.
0.01480
0.01280
0.01053
Gins. CisHmOu
Sn 100 Gms.
q. Solution.
30.12
47.89
48.57
dtt of
Aq. Sol.
1. 129
1.220
1.223
Abs. Coef. $
at IS*.
0.01090
0.00785
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.)
46i
MXTBOOSN
SoLUBniry of Nitrogen in Methyl Alcohol Solutions of Potassium
Iodide and of Urea.
(Levi, 1901.)
Solvent. Solubility of N (in terms of the Ostwald Solubility Expression /).
Ms*'
Cms. KI or of Urea
At IS*.
C^HSolution. ^» oi Solvent. l^. ^ iu <rf Solvent. /|».
At 25*.
"" da of Solvent. l^.
O (-puieCH^OH) 0.8080 0.2154 0.7980 0.1923 0.7937 0.1649
2.152 Kl O.8171 0.2028 0.8070 0.1802 0.8019 0.1524
3.053 " 0.8249 0.1966 0.8015 0.1756 O.810I 0.1466
10.939 " 0.8930 0.1676 0.8841 0.1464 0.8801 0.1258
2.738 Uien 0.8148 0.2030 0.8050 0.1823 0.7997 O.1561
4.841 ** 0.8231 O.1951 0.8122 0.1750 0.8080 O.1491
7.377 " 0.8350 0.1878 0.8241 0.1690 0.8193 0.1444
Solubility of Nitrogen in Ethyl Ether.
(Christoff, 19x2.)
Results in terms of the Ostwald expression / (see p. 227) , k ■ 0.2580, lu ■ 0.2561 ,
riTB
OOEN OXIDE (ic) NO.
Solubility in Water.
(Winkler, 1901.)
f.
^. ^'.
ff. f.
^.
^.
ff.
0
0.0738 0.0734
0.00984 40
0.0351
0.0325
0.00440
s
0.0646 0.0641
0.00860 50
0031S
0.0277
0.00376
10
0.0571 0.0564
0.00757 60
0.0295
0.0237
0.00324
IS
0.05x5 0.0506
0.00680 70
0.0281
0.019s
0.00267
20
0.0471 0.0460
0.00618 80
0.0270
0.0144
0.00199
25
0.0430 0.0419
0.00564 90
0.0265
0.0082
0.00114
30
0.0400 0.0384
0.00517 100
0.0263
0.0000
0.00000
For values of $, ff and g,
, see Ethane, page 285.
S(».uBiLiTY OF Nitric Oxide in Aqueous Sulphuric Acid S<^trriONs
AT i8^
(Lunge, 1885; Tower, 1906.)
Wt.
per cent HflS04
m Solution.
Sp.'Gr.
Teiuionof
Solubility Coeffic
of NO at 18
•t 15*.
B«0 Vapor.
98
1.84
« • •
0.0227
90
1.82
O.I mm.
0.0193
80
1-733
0.4 "
O.OII7
70
1. 616
1.5 "
O.QII3
60
I 503
3.1 "
O.OI18
so
1-399
6.2 "
0.0x20
(0.035, L.)
(0.017, L.)
* Volume of NO (at 760 mm.) per x volume of aqueoua HflSO«.
Solubility of Nitric Oxide in Alcohcx..
(Bunaen.)
o 5 10 . 15 20 24
0.316 0.300 0.286 0.275 0.266 0.261
absorbed by i vol. Ale.
* At o* and 760 mm.
Data for the solubility of nitric oxide in aqueous solutions of FeSOi, NiS04,
C0SO4 and MnCU at 20** are given by Usher (1908); HOfner (1907) and Man-
diot and Zecheulmayer (1906).
The abs. coef. /9 for N in sat. aq. NiS04 at 20* is 0.0245; for sat. C0SO4 it ir
0.0288 and for sat. aq. MnClt it is 0.0082.
Vols. NO*
NITROOEN OXIDE 462
NITROUS OXIDE NtO.
Solubility in Water.
(BuDflen; Roth, 1897; Knopp, 1904; Geffcken, 1904.)
Coefficient of Abeoiptioii fi
* • -A.
ff.
Solubility in Terms of Osttvmld
Expression (/).*
(B.)
(R.)
(R.)
(K.)
(G.)
S I 0954
XO 0.9196
15 0.7778
20 0.6700
25^ 0.5961
I . 1403
0.9479
0.7896
0.6654
0.5752
0.205
O.171
0.143
0.121
0.104
X.161
0.9815
0.8315
O.7131
0.6281
• • •
• • •
• • •
0.6739
• . .
1.067
0.9101
0.7784
0.6756
0.5943
•
Calculated by Geffcken.
For definitions of fi and q, 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.
(Lunce — Ber. 14, az88, '81; aee also Gcffcken's results.)
Sp. Gr. of HjSOi 1 .84 1 .80 1 . 705 1 .45 1 .25
Vols. N,0 dissolved
by 100 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. N,0.
100 vols, of NaOH solution of i.io Sp. Gr. absorb 23.x vols. N,0.
Solubility op Nitrous Oxide in Aqueous Solutions op Acids.
(Geffcken.)
Results in terms of the Ostwald Solubility Expression (/). See p. 227.
In Hydrochloric Acid. In Nitric Acid. In Sulphuric Acid.
Cms. HQ NaO piasolved Gms.HNOj NaO Disaolved Gms. HsSO* N>0 IXseolTed
per Liter. /j,. i^, per Liter. i^^, ^. per Liter. j^. ^.
18.22 0.755 0.577 36.52 0.777 0-S97 24.52 0.734 0.566
36.45 0.738 0.568 63.05 0.777 0.602 49.04 0.699 0-S43
72.90 0.716 0.557 126. zo 0.775 0.611 98.08 0.645 0.509
147.12 0.602 0.482
196.16 0.562 0.463
Solubility op Nitrous Oxide in Aqueous Solutions op:
t«
(Roth.)
Phosphoric Acid.
Coeflkient of Abs. in HsPOa Solutians of
t
Oxalic Acid.
Coefficient of Abfl. ia
CCOOH)s Solutioos of:
5
10
IS
20
as
I 057
0.8827
0.7388
0.6253
0.5427
4.73%. 8A4%. 9.89%.
1.0365 0.9883 0.9635
0.8665 0.8296 O.810I
0.7258 0.6977 0.6826
0.6147 0.5926 0.5810
05329 0.5143 0.5054
13^5%.
O.917I
O.77II
0.6505
OSSSS
0.4860
' o.8xa%. 370%.
I. 1450 I. 1094
0.9526 0.9264
0.7940 0.774s
0.6694 0.6538
0.5784 0.5643
463
NTTBOnS OXIDE
Solubility op Nitrous Oxidb in Aqueous Solutions op Propionic
Acid at 20^.
(SLnopp.)
Gms. CACOOH
per liter ^S-'^S
Coef . of Absorp-
tkm of N,0 0.6323 0.6369 0.6504 0.6534 0.7219
60.42 158.4 176.6
344.0
Solubility op Nitrous Oxide in Aqueous Salt Solutions.
Results by Geffcken in terms of the Ostwald expression (/). See
page 227
Sftlt.
Ammonium Chloride
Ammonium Chloride
Caesium Chloride
Lithium Chloride
Lithium Chloride
Potassium Bromide
Potassium Bromide
Potassium Chionde
Potassium Chloride
Potassium Iodide
Potassium Iodide
Potassium Hydroxide
Potassium Hydroxide
Rubidium Chloride
Rubidium Chloride
Fonnula.
Cone, of Salt per Uter.
SoiuhOit:
F of NsO.
GnunEquir.
Grams.
' /...
/»
NH«C1
O-S
26.76
0.730
0557
NH«C1
I.O
S3 52
0.691
0.529
CsCl
O-S
84.17
0.710
0.544
LiCl
OS
21.24
0.697
0-535
LiCl
i.o
42.48
0.623
0.483
KBr
0.5
59 -SS
0.697
0.536
KKr
1.0
119. II
0.627
0.485
KCl
OS
37-3
0.686
0.527
KCl
I.O
74.6
0.616
0.475
KT
O-S
83.06
0.702
0.541
KI
1.0
166.12
0633
0.492
KOH
o-S
28.08
0.668
0.514
KOH
1.0
56.16
0.559
0.436
RbCl
o-S
60.47
0.695
0.533
RbCl
1.0
120.95
0.625
0.483
Results by Knopp, in terms of the coefficient of absorption. See
page 227.
Sak.
Fonnula.
Cone, of Salt per liter. Cocf . of Afaaaradoi
KormaUty. Grams.' <* ^iP *t ao".
Potassium Nitrate
KNO,
O.I061
10.74 0.6173
((
it
0.2764
27.94 0.6002
<(
it
0.5630
56.97 0.5713
it
li
I. 1683
118. 2 0.5196
Sodium Nitrate
NaNO,
01336
11.37 0.6089
a
((
03052
25 -97 0.5876
a
U
0.6286
53 50 0.5465
••
•
li
I. 1200
95 30 04926
Results by Roth, i
in terms of the coefficient of absorption.
GfamsNaaper
Coefficient of Absorptiao eC N^O at:
100 unum ^^
SahilfaD.
^.
iof».
l^. iC^. srf^
0.99 I
.0609
0.88x9 0
.7339 0.O19X 0.5363
1.808 I
.0032
0.8383 0
.7026 0.5962 0.5190
3.886 0
•9131
0.7699 0
.649s 0.5520 0.477s
5.865 0
.8428
0.7090 0
.5976 0.5088 0.4424
NTTBOnS OXIDE
464
Solubility op Nitrous Oxidb in Aqueous Salt Solutions.
•
Results by Gordon in terms of coefficient of absorption. See p. 227.
Concentration of Sah.
Coefficient of Abiorpdon of NtO at:
SaU.
Cakium Chloride
tt
Lithium Chloride
it
St
Lithium Sulphate
u
Giams per
xoo Grams
Solution.
s
9
I
3
II
2
5
8
Magnesium Sulphate 5
7
Potassium Chloride
(C
(t
€i
Potassium Sulphate
it
Sodium Chloride
((
a
Sodium Sulphate
a
ti
Strontium Chloride
it
tt
10
4
7
14
22
2
4
6
8
12
5
8
12
3
S
13
79
86
99
35
8S
48
37
46
56
90
66
78
90
64
58
08
62
78
20
88
78
76
53
44
31
73
24
Gram
Mob.
per liter.
0.547
0.964
1. 416
0.319
0.928
2.883
0.219
0.521
0.836
0.521
0.687
0.997
0.676
I 037
2.147
3 414
0154
0.285
1. 107
1. 614
2.391
0.427
0.646
0.974
0215
0.380
0-939
5*.
0.819
0.668
0.510
0.986
0.878
0.606
0.934
0.795
0.646
0.766
0.708
0569
0.879
0.799
0.654
0.544
0.986
0918
0.800
0.713
0.634
0.808
0.692
0.559
0.928
0.848
0.644
xo".
0.697
0.586
0.441
0.831
0.743
0.512
0.792
0.665
0.555
0.664
0.586
0.491
0.751
0.693
0.574
0.459
0.831
0.763
0.682
0.603
0.532
0.677
0.574
0.486
0.788
0.709
0.547
0.591
,0.509
0.380
0.700
0.629
0437
0.670
0.557
0.477
0.561
0.488
0.417
0.643
o 591
0.500
0.390
0.701
0.637
0.585
0.510
0.449
0.584
0.482
0.417
0671
0.610
0.463
0.500
0.435
0.328
0.594
0.536
0.382
0.569
0.474
0.415
0.471
0.414
0.346
0.555
0.494
0.430
0.339
0.605
0.542
0.509
0.434
0.386
0.495
0416
0.354
0.578
0.550
0390
Solubility op Nitrous Oxide in Alcohol and in Aqueous Chloral
Hydrate Solutions at 20-.
(Bunacn; Knopp — Z. phyaik. Ch. 48, xo6, '04.)
In Aq. Chloral Hydrate (K.).
-A. , ^
Gms.
In Aloohd (B.).
Vola.NsO
t ^. (at o** and 760 mm.)
per X Vol. Alcohol.
o 4.178
S 3844
10 3.541
IS 3.268
20 3 .025
24 2.853
Normality
CiHClaOJ3iO.
0.184
0.445
0.942
1.165
1.474
1. 911
CsHCUOJIiO
per liter.
30.43
73.60
155-8
192.7
243.8
316.4
Coef. of
Aba. of NiO.
0.618
0.613
0.596
0.589
0.579
0.567
Solubility op Nitrous Oxide in Petroleum. Coefficient of
Absorption at io** « 2.49, at 20° — 2. 11.
(Gniewau and Walfisz — Z. physik. Ch. x, 70* '87O
465 NITBOnS OXIDE
Solubility op Nftrous Oxide in Aqueous Solutions op Glycerol and of Urea.
(Roth, 1897.)
Coefficient of Absozption of NjO in Glycerol Solutions of:
& .
3.46 Per cent. 6
73 Per cent, za.xa Pef cent. z6
^
.24 Per cent.
5
1.097
I -055
0.999
0.959
10
0.917
0.887
0.841
0.810
IS
0767
0-745
0.710
0.686
30
0.647
0.630
0.605
0-585
2S
0556
0.542
0.527
0.508
••.
Coefficient of Absorption of NsO in
k Urea Solutions of:
r-
3^z per cent. 4^7 per cent.
<)^7 per cent.
7.30 per cent.
9.97 per cent.
5
I
.104
1.096
1.088
I.IOI
1.069
10
0
.921
0.920
0.909
0.921
0.901
IS
0
.771
0-773
0.761
0.772
0.761
ao
•
0
•653
0.656
0.644
0-655
0.651
as
0
•569
0.567
0.559
0.570
0.569
Solubility of Nitrous Oxide in Aqueous Solutions of Glycerol.
(Henkel, 1905, 19x2.)
Results at 15*^. Results at 20®.
Per cent Glycerol. Absorption Coef . a. Per cent Glycerol. Absorption Coef . ce.
o 0.7327 o 0.6288
2.49 O.7181 2.36 O.613I
3.28 0.7103 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 0.5315
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 Creighton (1910-11).
NITBOaiN TETBOXmS NOi.
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 NOi + NO by v. Wittorff (1904), and for mixtures of Nft + 0 Nitrotoluene
by Breithaupt.
NITBOCELLUL08E (Soluble Pyroxylin, Tetra and Penta Nitrate).
Solubility in Ether-alcohol Mixtures.
(Matteoschat, 1914; see also Stepanow, 1997.)
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 de^red com-
position of solvent was added. Lower results were obtained with ready prepared
ether-alcohol mixtures.
Ratio of GtoA. Gun Cotton Dissolved per xoo Gms. Solution in Mixtures Prepared with:
Ether : AkohoL 99.5 Vol. % Alcohol. 95 Vol. % Alcohol. 90 Vol. % Alcohol. 8oV61.%Alcohd.
X • 2 34 *4 ••. •.• ••■
x:i 52.3 42.3 28.7 14.2
2-1 40.5 52.4 53-9 45
3:1 25 42.4 S3 575
NOVOCAINE
466
NOVOCAINE (baae) CH,(aH4NH,COO)CH,[N.(C,H,)d.2Hrf).
100 cc. H|0 dissolve 0.333 gm. anhydrous novocaine at 20**. (Zaiai. 19x0.)
100 cc. oil of sesame dissolve 4.29 gms. anhydrous novocaine at 20^.
NOVOCAINE (Hydrochloride) CH,(C«H4NH,C00).CH,[N(CtH*)J.HCL
100 gms. H|0 dissolve about 100 gms. of the salt at room temp.
. 100 gms. alcohol dissolve about 3 gms. of the salt at room temp.
ANE CH,(CH,)tCH,.
REaPROCAL Solubility
OF
Octane and
Phrnol.
(Campetti and Del Groaso, 19x3.)
f.
Gms. Phenol per
f.
Gms. Phenol per
xoo Gms. Mixture.
xoo
Gms. Mixture.
22.55
13.28
49.Scrit
. t.
52.2
37.85
22.74
49-35
52.37
38.15
23.53
44.7
71.14
44.70
32.85
30.65
82.01
47. 75
41.72
19.65
85.99
OLEIC ACm CbHi7CH:CH(CH,)7COOH.
Solubility of. Oleic Acid in Aqueous Alcohol Solutions at 25*.
(Seidell, 19 10.)
Oleic acid oi dn — 0.8035 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. % QHiOH 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. %
CsHiOH the following results were obtained:
Wt. Per cent
QH»OH.
SI
58.2
65. S
70.2
81.4
cc. Oleic Add per
xoo cc. Aq. Alcohol to
produce doudineas.
Remarks.
0 . 08 — 0.2 Qoudiness gradually increased.
0.2 —0.4
0.3 — 0.6 Qoudiness disappeared when about 5.5 cc add had been added.
0.6 —I " " " " 4.5 cc " " " "
00 No doudiness 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 b
changed to addition of HsO to mixtures of oleic acid and alcohol. By this method
perfectly clear liquid may be transformed by one drop of the HjO 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
Opalescent Mixtures.
Alcohol + Oleic Add Mixture.
Results Calculated from the
Plotted Curve.
CAOH.
Oldc Add.
15-30
1.794
15-30
3-588
15-30
4-485
15-30
7-175
15-30
II. 210
24.42
22.420
15-30
20.810
I -195
8.969
H^ Added
Wt. Per cent
cc. Oleic Acid
Gms. Oleic Ad
to Cause
QILOHin
Aq. Alcohol.
per TOO cc.
per xoo Gms.
Separation.
Aq. Alcohol.
Sat. Sal.
10.4
57
• • •
0
10.2
58-5
0
5
9.8
60
II
12.3
925
62.5
30
20
8.05
65
49
30. s
10.10
67-5
69
40
6.50
70
91-
so
0.321
75-5
• . •
68.5
80
...
88
After standing 24 hours the opalescent mixtures separated into layers which,
on analysis, gave the results shown in the following table.:
467
OLEIC Acm
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:
Wt.%
amOH
■> r
oc. Aq.
Alcohol
Alc.u2ii. M^""-
70.2
70.2
65.5
70.2
70.2
70.2
25
25
26.5
25
25
35
oc.
Oleic
Add.
2
4
5
8
12.5
25
oc.H|0
to Cause /-
Sepan- ^cc. Total
Lower Layer.
tion.
3.90
3.70
1-75
2.75
1.55
I
Vol.
29
26
22.7
16
6
4.5
Sp. Gr.
0.893
0.890
0.891
0.893
0.890
\t
oc Oleic cc. Total
Upper Layer.
K
Add.
1.48
1.89
1.93
0.98
0.37
0.28
Vol.
I
6
9.3
19
33.2
55.5
Sp. Gr.
• • •
0.875
0.875
0.876
0.878
0.877
oc. Oleic
Add.
0.35
1.98
2.78
6.59
11.87
24.14
The CsH«OH in the two layers could not be determined on account of excessive
foaming during distiHation 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.)
Q^i„^4 Gm». Oleic Add per xoo
^'^t- Gms. Sat. SbT
Water less than o. i
5% Aq. Solution of Bile Salts about o. 5
5 % Aq. .Solution of Bile Salts+ 1 % Lecithin 4
Distribution of Oleic Acid between Aqueous Alcohol and Benzine. (Holde/xo.)
Strength of Aq.
Alcohol in Vol.
Per cent.
84.1
76.9
63.7
50.5
42.4
Gm. (Approx.) of Oldc Add in:
A ■
50 CC. Aq. Alcohol
Layer.
0.277
O.II2
0.025
0.006
0.002
50 CC. Benzine Layer.
Layer.
0.723
0.888
0.975
0.994
0.998
Dist. Coef.
2.61
7.93
39
166
499
Solidification-points of Mixtures of Oleic and Stearic Aaos. (Meidrum/zj.)
Solidification Per cent Oldc Add Solidification Per cent Oleic Acid
Temp. in Mixture. Temp. in Mixture.
o 54-8 50 44.7
10 53.3 60 41.2
20 51.6 70 36.6
30 49.7 80 30.5
40 47-6
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 (19 12).
TriOLEIN (Ci»H«0,)iCiH5.
Sca.IDIFICATION-POINTS OF MIXTURES OF TRIOLEIN AND OtHER FATS.
(Kremann and Schoulz, 19x2.)
Friolem + Tnpalmitm.
f. Wt. Per rent
Triolein + Tristearm.
Tnpalmitm + Tnsteann.
A. Wt. Per cent.
* • Triolein.
*. wt. Per cent
*' Trifltearin.
Triolein.
— 7 100
+ 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
so 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 0
56 0
54.5 31.2
Data for the ternary system, triolein,, tripalmitin and tristearin are also given.
OILS
468
OILS. (See also Fats, p. 303.)
Solubility of Several Oils in Alcohol (du « 0.795) at 14-15^.
(Davidflohn and Wnge^ Z9XS-)
Gnu. Oil per xoo Gnu.
Sat. SoL
OU.
Linseed Oil
Rape Oil
Cotton Seed Oil
Olive OU
3.32
1.36
3.61
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 bv Aubert (1902). Nigella oil, 4.3;
oil of boldo leaves, more than 100; matico oil, about 20; cascarilla oil, 5; weld-
mint oil, 66.
Misdbility 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;.
OSBIIC ACID OsOi, 100 gms. HtO dissolve 5.88 gms. Osmic Acid at about 15*.
(Squire and Coines, 1905.)
OXAUC ACm H,C,04.2H,0.
Solubility in Water.
(Koppel and Cahn, 1908; for older data see Alluard, Miczynski, z886; Lamourooz, 1899.)
Gnu. Ha'
zoo Gnu.
8.69
12.46
17.71
23.93
30.71
37.92
45.80
54.67
H1C1O4.2H1O melts in its HtO of crjrstallization at 98®.
Solubility of Oxalic Acid in Aqueous HCl and in Aqueous HN0« at 30*.
(Mosson, 19x2.)
In Aq. Hydrochloric Acid.
f.
Gms. HiCfii
zoo Gms. Sat.
per
Sol.
SoUd Phase.
f.
— 0.064
0.1805
Ice
20
— 0.152
0.452
It
30
- 0.533
1.820
It
40
— 0.936
3.291
II
50
- 1.50
S.836
«
60
- 0.95
3 302
H«Q0«.3H«0
70
0
3.416
<i
80
+10
5.731
11
90
t. Sol.
Solid Phase.
H^QA-a^O
If
f<
M
G. Mols.
HQ
per liter
Sat. Sol.
O
0.503
0.970
1.939
2-959
4- 528
6.026
7.907
9.680
(fa. Sat.
SoL
•0594
.0561
■0577
.0654
•0757
•0957
.1165
.1494
.1843
G. Mols.
(COOH),
Sx liter
t. Sol.
1.479
1. 190
1.032
0.821
0.675
0.555
0.525
0.607
0.871
Gms.
(COOH),
Sx liter
t. Sol.
133. 1
107. 1
92.85
73.88
60.74
49.95
4725
54- 63
78.38
G. Mols.
HKOi
per liter
Sat. Sol.
0.478
1.606
4.224
9- 590
13.62
14.12
15.59
16.92
20.84
21.63
In Aq. Nitric Acid.
G. Mols.
dLpSat.
Sol.
1.0648
1.0932
I. 1666
I . 3074
1.3938
1.4060
I. 4319
1.4443
I. 4819
I. 4917
(COOH)t
ST liter
t. Sol.
1.268
1.039
0.790
0.639
0.847
0.966
1. 114
0.840
0.524
0.553
Gms.
(C00H)t
Sir liter
t. SoL
114. 1
9348
71.09
57.50
76.23
86.94
100.2
75.6
47.15
49.76
Solubility of Oxalic Acid in Aqueous Solutions of HsS04 at 25®. (Wirth. *o8.)
Cone, of J ^ttu* Gms. per loo Gms. Sat. Sol. Cone, of j .« q.^ Gms. per zoo Gms. Sat. SoL
Aq. H^4 *» Sl,^*- . =- * . Aq. H.SO4 *• ^T** . rZ ^ n
Normality.
O
X
2.39
4.36
Sol.
1.047
1.064
1. 140
1. 146
S0i.
o
2.98
7.30
12.57
(COOH)i. Normality.
10.23 4.85
8.03 .5.67
6.02 6.45
4.26 8.9
Sol.
1. 157
1. 177
1.220
1.280
S0i.
14
16.44
17.84
25.92
(C00H)i.
3.92
3.51
3.12
2.37
469
OXAUC Acm
S(M«UBILITY OF OXALIC AciD IN SeVBKAL AlCOHOLS.
(Timofeiew, 1894.)
I
Gms. (COOH),
Cms. (COOH)t
Akobol.
f.
per xoo Gms.
Sat. Sol.
Alcohol.
f.
per xooGras.
Sat.SoL
Methyl Alcohol
- 1.5
34-2
Propyl Alcohol
- 1. 5
12.2
U It
+20.2
39.8
« «
+18.5
16.7
Ethyl Alcohol
- IS
22.4
(( tt
20.2
17.5
(( u
+18.5
26.2
Isobutyl Alcohol
20.2
10.9
tt t(
20.2
26.9
-
Solubility of Oxalic Acid in Absoluts and in Aqueous Ethbr at 25^
(Bddtker, 1897; Bouzgoin.)
100 gms. absolute ether dissolve 1.47 gms. (CC)OH)i.2HtO.
100 gms. absolute ether dissolve 23.59 gms. (CC)OH)t.
In Aqueous Ether Solutions.
Gms. Solid Add Added per xoo cc Ether Solution.
Gms. per xoo cc. Ether Solation.
(COOH),.aB^.
(I)
(2)
5
5
5
5
5
5
5
5
5
S
5
(COOH),.
o
o
o
2.44
4.82
7.14
9.42
11.63
13 -79
18.18
22.73
H,0.
1.250
0.788
0.418
0.360
0.484
0.558
0.632
0.676
0.760
0.816
0.816
(COOH),.
0.742
0.720
1.044
3.388
6.038
8.538
10.996
13-316
15.684
17.818
17.818
(x) Ether satnimted with water.
(a) Ether containing 0.694 P^ cent water.
100 gms. glycerol dissolve i^ gms. oxalic acid at 15.5^. (Ossendowski, 1907.)
100 gms. 95% formic acid dissolve 9.74 gms. anhydrous oxalic acid at 16.8^.
(Aschan, xgxj.)
DiSTKIBUTION OF OXALIC AOD BETWEEN WaTER AND AlfYL AlCOHOL AT 20^
(Hers and Fischer, 1904.)
Milllmols \ (COOH), per xo cc
^ II A
Gins. (COOH), per xoo cc.
Aq. Layer.
0.6806
2.364
6.699
10.029
Alcoholic Layer.
O.1451 '
0.7233
2.550
4.300
Aq. Layer.
p. 306
1.064
3015
45"
Alcoholic Layer.
0.0653
0.326
1. 148
. 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, xgxs.)
Results at 15"*. Results at 27^
Sm. Mob. (COOH), per Liter.
Dist. (
0)ef. of:
Qta, Mob. (CppH), per Liter.
Dist.
Coef.of:
Water
Ether
Total
Undisaoc
Water
Ether
Total
UndiaaocT
Layer.
Layer.
Add.
Add.
Layer.
Layer.
Add.
Add.
0.343s
0.02945
II. 6
8.49
0.760
0.0637
II. 9
8.18
0.1885
0.01395
13.5
8.81
0.561
0.0433
13
8.37
0.124
0.00845
14.8
8.69
0.3S75
0.0250
14.3
8.26
0.0892
0.00553
16. 1
8.72
0.2550
6.0165
IS. 5
8.12
0.0470
0.00248
19
8.19
0.1754
0.01025
17. 1
7-94
0.0435
0.0022
19.8
8.26
Data for the effect of HsSOi upon the above distribution are also given.
Data similar to the above for a greater range of cone, at 35* are given by
Chandler (1908).
OZTOEN 470
OZTGKN Q^
SOLUBILITT IN WaTBR. (WinUer. 1891; Bohr and Bock, 1891O
%• Coef . fli Abwcpdon ^. q, Ute?^. **• Coef . of Abyrpdoa ^. f,
o 0.048^ 0.0496! 0.00695 zo. 187 40 0.0231* o.o333t 0.00508
5 0.0429 0.0439 0.00607 8.907 50 0.0209 0.0207 0.00266
10 0.0380 0.0390 0.00537 7.873 60 0.0195 0.0x89 0.00227
Z5 0.0342 0.0350 0.00480 7.038 70 0.0183 0.0x78 0.00x86
20 0.0310 0.0317 0.00434 6.356 80 0.0176 0.0172 0.00138
25 0.0283 0.0290 0.00393 5-77^ 90 0.0172 0.0169 0.00079
JO o.oa6i 0.0268 0.00359 5.255 100 0.0170 0.0x68 0.00000
«W. tB.andB.
For values of fi and q aee Ethane, p. 385.
According to determinations by Fox (x9o9a), which Bgftt tatiduianiy with the abonrB, the aohiUUty
of <n3rgen in water u ezpreseed by the formula:
1000 X aba. coef. 0 — 49-339 — i'3440 1 + 0.28752 1> — 0.000303^ #.
References to more recent papers on the solubili^ of oxygen are given by Coslie (i9i7f I9i$)*
Solubility of thb Oxygen of Air in Water.
ۥ. S'**- S-6s*. 14- 78*. 84. 8*.
Solubility* 8.856 8.744 7.08 5.762
* oc. Oxygen per looo cc. H|0 aatucated with air at 760 mm.
Solubility of Oxygen in Water and in Aqueous Solutions of Acids,
Bases and Salts. (Geffcken, 1904.)
Aq. Solutioa of: Cuuctutratioii
per Liter.
SdubOityo
f Oxygen.*
CramEquiv
^ Grams.
/!»•.
/is.
Water alone
• a •
• • •
00363
0.0308
Hydrochloric Acid
O-S
18.22
0.0344
0 .0296
n
i.o
36.45
0.0327
0.0287
u
2.0
72.90
0.0299
0.0267
Nitric Acid
OS
36.52
0.0348
0.0302
tt
1.0
63 05
00336
0.0295
it
2.0
126.10
00315
0.0284
Sulphuric Acid
OS
24.52
00338
0.0288
<i
1.0
49 04
0.0319
00275
u
2.0
98.08
00335
0.0251
u
'3-0
147"
0.0256
0.0229
tt
4.0
196.16
00233
0.0209
It
S-o
245 ■ 20
0.0213
0.0194
Potassium Hydroxide
OS
28.08
0.0291
0.0252
it
1.0
56.16
00234
0.0206
Sodium Hydroxide
o-S
20.03
0.0288
0-0250
((
1.0
40.06
0.0231
0.0204
tt
2.0
80.12
00152
00133
Potassium Sulphate
OS
43-59
0.0294
0.0253
it
I.o
87.18
00237
0.0207
Sodiimi Chloride
o-S
29.25
0.0308
0.0262
it
1.0
585
0.0260
0.0223
It
2.0
119 .0
0.0182
0.0158
* In terms of the Ostwald Solubility Expression. See page 917,
Solubility of Oxygen in Aqueous Potassium Cyanide Solutions at 20*.
(Maclaurin, 1893.)
Gms. KCN per loo gms. sol. i lo 20 30 50
Coefficient of absorption /3 0.029 0.018 0.013 0.008 0.003
471
Sqlubilitt of Oxygen in Sea Water.
(Fox, 1909a.)
OZTGKN
Before using the sample of sea water for the solubility determinations, it was
found necessary to add acid, otherwise the COs 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 ^
+ 0.006009 ^ + 0.0000632 ^ — CI (0.1161 — 0.003922 1 4-0.0000631 fi).
PutsChloriiie
per xooo.
f-o».
4*.
8*.
la*.
x6».
ao*.
ur
a8*.
0
10.39
9.26
8.40
7.68
7.08
6.57
6.14
5.75
4
9.83
8.8s
8.04
7.36
6.80
6.33
5.91
5.53
8
9.36
8. 45
7.68
7.04
6.52
6.07
567
5.31
12
8.90
8.04
7.33
6.74
6.24
582
5.44
5.08
16
8-43
7.64
6.97
6.43
5. 96
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 (191 1).
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.
S(H.uBiLrrY OF OzTGEN IN Aqubous Salt Solutions at 25^.
(MacAithur, 19x6.)
i<
«
II
II
11
Aq. Salt
Solution.
Dist. H^
o.i25»NH4a
0.25 n
X n
o.X25nBaClt
0.25 n
0.50 n
X n
0.25 nCadi
I #1 "
5 n "
o.i25n Cad
0.1 25 nua
0.50 n
1 fi
2 n "
3 i» "
4 n **
o.Z25nMgCl|
0.50 n
1 n
2 n "
4 « "
5 «• "
dUAq. ccozy-
Solu- gen per
tion. Liter.
M
M
(I
II
I
I.OOIS
1.0025
1. 014
1. 019
1.042
1.082
I.X77
1.022
1.084
1.34
Z.014
1.0004
Z.0091
1.02 1
1.044
I.I 13
1.220
1. 01 1
1.044
1.085
1. 160
1.284
1.343
S.78
2.31
1. 16
0.07
5.40
5.04
4.27
3.10
5.08
371
2.14
5.67
563
S.17
4.59
3.63
1.97
1. 12
5.35
4.37
3.18
2.22
0.78
0.54
Aa.Salt
Solution.
0.25 »KBr
2 n "
4 » "
o.i25»Ka
0.25 » "
0.50 » "
1 n "
2 #1 "
3 n "
4 » "
o.X25nKI
0.25 n "
0.50 n "
X » "
2 » **
5 n "
0.25 nKNOb
0.50 n "
in"
2 « "
o.i25nK|.S04
0.25 n "
O.S n "
o.i25nRbCl
(^ Aq. ocOzy-
Solur geni
tion. lit
per
iter.
1. 019
1.079
1. 162
1.003
1.0086
X.020
1.042
1.086
1.134
1. 170
1. 013
X.027
1.056
1.116
1.23
1.46
I.015
1.029
1.059
X.IIO
1. 016
1.032
1.060
1.0094
S.29
3-27
X.84
5-52
5.30.
4.98
4.26
3-21
2.36
X.86
5-65
5-49
5.20
4-75
3-77
1. 81
549
5"
4.61
3.65
5."
4.66
3.89
S.65
Aq. Sah
SoIuti<».
o.i25n
0.25 n
0.50 n
X n
NaBr
2
3
4
6
n
n
n
n
II
II
II
II
II
II
II
O.I25»
0.25 #1
0.50 n
X n
2 n
3 *»
4 n
0.1 25n
0.25 n
0.50 n
1 n
O.I25»
0.25 n
0.50 n
X n
2 fi
NaG
<i
11
II
II
II
II
NatSO«
II
II
11
Sucrooe
II
M
II
U
dig ot oc. Ozy-
Sohi- gen per
tion. Liter.
X.007
X.017
1.036
1. 07s
1. 150
1. 219
1-305
1.455
X.0022
X.0067
X.017
X.038
1.075
1. 1X2
I.I49
1. 014
1.032
1.063
I.I3O
I.OI5
1033
I ^.5
1.147
1.336
5.65
5.52
5.15
4.47
3-37
2.57
2.02
1.28
5.52
530
4.92
4.20
3.05
2.24
1.62
5-04
4.60
3.97
3
5.40
4.82
4.39
3-20
1.84
0X70KN 473
Solubility of Oztgbm in Aqueous Sulfuric Acid Solutions.
Results at 2I^ (Bohr, 191a) Results at 20^ (Christoff, 1906).
NoRDftlity of
Abwrp.
NonaaUtyof
AbMtp.
S*v7»
Ostwald Sduhility
H^SOf
Coef.^
HaSOi.
Coef.^.
H.SO4.
0
0.0310
34.8
0*.0I03
0
0.03756
4.9
0.019s
39.6
O.OII7
35-82
O.OI815
8.9
o.oiss
34.3
0.0201
61.62
0.01407
10.7
0.0143
35. 8 (-96%)
0.027s
95.60
0.03303
20.3
O.OII9
Solubility of Oxtgbn in Ethyl Alcohol, Mbthyl Alcohol and
in acbtonb.
CnmoleJeir^Z. pbjnik. Ch. 6^ 15x1 '00; Levi — Gazs. chim. iuL 31, lit 513, 'oxO
f.
In Ethyl Aloohbl of
90-7* (T.).
InMethvl
Alcohol (LO
la AceCone (L4
0
0.2337
0.2297
0.31864
0.2997
5
0.2301
0.2247
0. 30506
0.283s
zo
0.2266
0.2194
0.29005
0.2667
IS
0.2232
0.2137
0.27361
0.2493
20
0.2201
0 . 2073
0.25574
0.3313
as
0.2177 (24^
0.2017
(24^0
0.23642
0.2127
30
• • .
• . •
0.21569
0.193s
40
• • •
• • •
0.16990
0.1533
SO
• • •
• • •
0 . I 1840
0.1057
For values of 0 and fi\ see Ethane, p. 285. / « Ostwald Solubility Expres-
sion. See p. 227.
The formube expressing the solubility of oxygen in methyl alcohol and in aoe-
toQe as shown in the above table are as follows:
In Methyl Alcohol / » 0.31864 — 0.002572 / — 0.00002866 fi.
In Acetone / — 0.2997 — 0.00318 / — 0.000012 fi.
The formula expressing the absorption coefficient of oxygen in ethyl alcohol
is /J "= 0.23370 — 0.00074688 1 + 0.000003288 fi.
Solubility of Oxygbn in Aqubous Alcohol at 20^ and 760 mi.
(Lubaxach, 1889:)
Wt. Per cent Vol. Percent Wt. Percent Vol. Percent Wt. Percent Vol. Percent
AkohoL Absorbed O. Alcohol. Absorbed O. Alcohol. Absorbed O.
o 2.98 33.08 2.52
9.09 2.78 28.57 2.49
16.67 2-63 33.3^ 2.67
Solubility of Oxygbn in Pbtrolbum. Coefficient op Absorption at
10** = 0.229, AT 20** = 0.202.
(Gniewux and Walfisz, 1887.)
Solubility of Oxygen Ethyl Ether.
(Christoff, 191 3.)
Results in terms of the Ostwald Solubility Expression, k » 0.4235, ho ■
04215,
so
3 SO
66.67
4-9S
80
S.66
473
OZTGKN
Sglubility of Oxygen in Aqueous Solutions of:
Qiloral Hydrate act so"*.
Gnu.
Ca«.CH(0H). «i«o£
per loo Gmft. Aq. Sok
Aq. SaL
16.9
52.9
61.08
71.4
73
1.0798
I . 1630
1-2935
I -354
1.382
1.4404
1.46
(MOUer, 1913-13.)
AbB. Coef . fi
(Bunsen)
atao*.
o*. 0279s
0.0249s
0.0232s
0.02410
0.02580
0.02730
0.03280
Glycerol at 15*. (Mailer, x9ia-x3.)
Gms.
(CH^H),CH0H d of
per xoo Gms.
Aq. Sol.
20.5
25
37-3
45
52
71.5
88.5
Aq. SoL
dl2.6 =1.0509
du =1.0621
di4.6=i.o9S7
^U-6=^I*Il6l
du.6=i.i3Si
(f 12.6 ==1.1908
dl8.6=1.236
Abs. Coef. 0
(Bunsen)
at 15*.
0.02742
0.02521
0.02022
0.01744
0.01570
0.00950
0.00886
SoLUBiLirY OP Oxygen in Aqueous Solutions of:
d^of
I Aq. Sol.
Glucose at 20^. (Mailer, xgxa-ia)
Gms. C4I^
per 100 Gms.
Aq. SoL
10.84 1-0413
20.7 1.0835
33.8 I. 1370
51.9 1.229s
58.84 1.2649
Abs. (>)ef . 0
(Bunsen)
at ao*.
0.02690
0.02250
0.0x815
0.01390
0.0x250
Cane Sugar at 15
Gms. CttHfAi
per xoo Gms.
Aq. Sol.
du of
Aq. SoL
12. 1
24.38
28.44
42.96
SO
1.0482
I . 1022
I.X20S
I . 1933
1.23x8
(MODer, x9x»-X3.)
Abs. Coef. /I
(Bunsen)
at xs*.
0.02969
0.02396
O.O2181
0.0x600
0.0x359
Influence of Anesthetics upon the Solubility of Oxygen in Olive Oil.
(Hamberser, x9xx.)
Name and 0>nc. of Solubility of Oxygen in;
Narcotic Added
to tbe Oil.
Sulfonal (0.8 per xoo)
it
Trional (saturated)
CI
Tetronal (s per xoo)
tt
Pure
Solvent.
9.69
9.69
9.69
9.10
9.10
9.67
9.67
8.53
Narcotic
Solution.
455
5.68
6.25
4. 55
5.68
9.10
9.20
7.96
Name and Cone, of
Narcotic Added
to tbe OIL
Monochlorhydrine (5
(a.S
(10
(S
(5
(a.S
ti
Solubility of Oxygen int
Pure Narcotic
Solvent. Solutidn.
xoo) 9.10 7.50
Dichlorhydrine
Phenylurethan
) 9.10
) 9- 10
) 9- 10
) 9- 10
) 8.53
) 8.53
7.50
7.90
.96
I
6.25
7.50
Camphor (xo per xoo)
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 mm. Hg, are given by Findlay and
Creighton (191 1).
OZONE 0i.
Solubility
IN
Water.
(von Mailfert, X894;
Carius; Schdne, X873)
f.
w.
G.
R.
f.
w.
(?.
R.
0
39-4.
61.5
0.641
27
13-9
SI -4
0.270
6
34.3
61
0.562
33
7.7
395
0.19s
II. 8
29.9
59-6
0.500
40
4.2
37-6
O.II2
13
28
58.1
0.482
47
2.4
31.2
0.077
IS
2S-9
S6.8
0.456
S5
0.6
193
0.031
19
21
S5-2
0.381
60
0
12.3
0
W ™ milligrams ozone dissolved per liter water,
one liter of the gas phase above the solutions. R
undissolved ozone (W -i- G),
G B milligrams ozone in
ratio of the dissolved to
OZONE 474
The experiments of Schdne (see preceding page) were repeated by Inglis
(1903). "The results confirm SchGne's experiments and indicate that ozone,
when passed through water, is partly decomposed."
According to Moufang (191 1) the solubility of ozone in distilled water ranges
from about 10 milligrams per liter at 2^ to about i .5 milligrams per liter at 28°.
The solubility is greatly affected bv other substances in solution. Small amounts
of acids increase the solubility and render the aaueous solution of the ozone more
permanent. Alkalis decrease the solubility. Neutral salts («.e., calcium sulfate)
mcrease the solubility.
Solubility of Ozone ik Dilute Sulfuric Acid.
(Rothmund, 191 a-)
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 HsS04 m which decomposition takes
place much more slowly than in pure water. At o^ the absorption coef. fi (Bun-
sen, see p. 227) in o.i n HsS04, 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
ffaseous. The solubility depression which ozone experiences through o.i n
HtS04 is calculated as 1.5%. Therefore, by extrapolation, it is calculated that
the abs. coef. fi of ozone in H|0 at o^, is 0.494.
PALLADIUM CHLORIDE PdCl,.
When I gm. of palladium, as chloride, is dissolved in 100 cc. of HsO and shaken
with 100 cc. of etiier, 0.02 per cent of the metal enters the ethereal laver at ord.
temp. When aq. 10% HCi is used,^o.oi per cent of the metal enters the ethereal
layer. (Mylius, 191 1.)
100 cc. anhydrous hydrazine dissolve i gm. PdCls, with evolution of gas and
formation of a black precipitate, at room temperature. (Webb and BrodeiBOQ, x9z50
PAUanC ACID CH,(CH,)i4C00H.
Solubility in Aq. and Absolute Ethyl Alcohol.
i (Fakiola, 19x0.)
Gms. CHa(CH«)MC00H per 100 cc:
• • Absolute Aq. 75% A
Aa. 75% Aq. <o%
Alcohol. Alcohol. Alcohol.
10 2.8 0.24 0.05
20 9.2 0.43 0.08
30 ... 1. 19 0.12
40 319 359 031
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.)
Gms.
Gm.5.
Alcohol.
f.
CH,(CH,)mC00H
per 100 Gms.
Sat. Sol.
Alcohol.
f.
CH,(CH,)urOOB
per 100 Gms.
Sat.SoL
Methyl Alcohol
0
0.72
Propyl Alcohol
0
2.92
((
21
S.I
u
21
13-8
tt
36
29s
Isobutyl Alcohol
0
2.2
Ethyl Alcohol
0
2
tt
21
12.8
«
21
10. 1
One hundred gms. of aq.-5% solution of bile salts dissolve about o.i gm. palmitic
acid. 100 gins. aq. 5% solution of bile salts containing i % of lecithin dissolve 0.6
gms. palmitic acid. (Mooce, Wilson and Hutchinaoo, 1909.)
475
PALBOnC Acm
Solidification Points of Mixtures of Palmitic and Stearic Acids.
(De Visser. 1898O
Fifty gram samples of each mixture were used and great care taken to insure
accuracy of the determinations.
rof
Cms. Stearic Acid
SoUdi-
per xoo Cms.
fication.
Mixture.
69.32
100
67.02
90
6451
80
61.73
70
58.76
60
f of
Gms. Stearic Add
fof
Gms. Stearic Add
Sotidi-
perxooGins.
SoUdi-
per xooGma.
fication.
Mixture.
fication.
Mixture.
57-2
ss
54.85 Eutec. 30
56.42
so
55-46
25
56.38
45
56.53
20
56.11
40
59 31
10
SS-62
36
62.62
0
Additional determinations on this system by Dubowitz (191 1) 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:
Palmitic Acid + Tripalmitin
4- " + Stearic Acid.
+ " + Tristearin.
-|- Tristearin + Stearic Acid.
-|- Tristearin.
Tripalmitin + Tristearin + Stearic Acid.
" -f Stearic Acid.
Palmitic Acid Cetyl Ester + Parafi&n.
II
II
II
II
(Kremann and Klein, 19x3.)
(Kremann and Kxopacb, 19x4.)
it
•I
•I
i«
«
It
(Kremann and Klein, 19x3.)
(Palazzo and Battelli, 1883.)
(SrhindrimriBfT, 1901.)
((3ori, 1913.)
PAPAVERINE C20H21NO4.
100 gms. carbon tetrachloride dissolve 0.203 gm. at 17^.
100 gms. carbon tetrachloride dissolve 0.518 gm. at 20^
100 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.;.*pipefidine, i.gm.; diethylamine,
0.4 gm. (Scholts, Z9X2.)
PARAFFIN.
Solubility of Ozokerite Paraffin of Melting Point 64^-65
Sp. Gr. at 20° = 0.917 IN Several Solvents at 20".
(Pawlewski and.Fikmonowicz, 1888.)
Gms. Paraffin per xoo
■" Solvent.
AND
Solvent.
Carbon Disulfide
Benzine, boiling below 75*
Turpentine, b. pt. isS'^-iG^*
Cumol, com. b. pt. 160*^
" fiac. i5o'*-i6o''
Xylene, com. b. pt. i35**-i43*
'' frac. ijs^'-isS**
Toluene, com. b. pt. io8*'-iio*
" frac. io8**-io9*
Chloroform
Benzene
Ethyl Ether
Isobutyl Alcohol, com.
Gms.
Solvent.
12.99
"•73
6.06
4.26
3-99
3-95
4.39
3.88
3-92
2.42
1.99
1-95
0.285
cc.
Solvent.
Acetone
8.48 Ethyl Acetate
S . 21 " Alcohol
3.72 Amyl Alcohol
3 . 39 Propionic Acid
3 . 43 Propyl Alcohol
3 . 77 Methyl Alcohol
3 . 34 Methyl Formate
3.41 Acetic Acid
3.61 " Anhydride
1 . 75 Formic Acid
. . . Ethyl Alcohol 75%
0.228
Gms. Paraffin per xoo
Gms.
— 1
cc.
Solvent.
Solvent.
0.262
0.209
0.238
• • •
0.219
• « •
0.202
0.164
0.165
• • •
0.141
• • •
0.071
0.056
0.060
• • •
0.060
0.063
0.025
• a •
0.013
0.015
} 0.0003
...
F.-pt. data for paraffin + stearin arie given by Palaz2So and Battelli (1883).
PBMTIHI
476
PENTIHI CH«(CHt)iCH«.
Data for the solubility of pentane in liquid carbon dioxide, determined by the
synthetic method, are given oy BQchner (1906).
IsoPSNTlHl (gH«)tCH.CHsCH«.
RbCIPROCAL SCH.UBILITY OF ISOPBNTANE AND PhBNCX.. (Cainpetti tad Dd Grano, 19x3.)
Gntt. Phenol per 100 Cms.
f.
Iioprntaiif Rich
Layer.
Phenol Rich
4
7
II
18
29
40
87
80
75. S
68
S8
50
20
30
40
50
60
66 crit. texnp.
F.-pt. data for muctures of hexachloro-a-£eto 7-i^-pentene, CiCUO, + penta
chloromonobromo a-keto y-R pentene, CiCUBrO, are given by Kilster (1890, 1891).
PIPTONE.
100 gms. HsO dissolve 42.2 gms. peptone at 20-25^ (Dehn, 1917.)
pyridine " 0.22 "
aq. 50% pyridine " 12.6 "
PIECHLORIC ACm HCIO4.
Solubility in Water, (van Wyk, 1903, 1905.)
Muctures of HCIO4 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. HGOi
Mob. HCIO«
«•. 1
per zoo Mols.
Solid Phase.
v.
per 100 Mob.
Solid Phaie.
HC10«+HA
HCIQ,+IV>-
0
0
loe
-32
26
HCK>«.>mo
— 10
5
M
-29.8
28.57
II
— 21
7
«
-44
27
HCK)«.9^0
-34. 5
9
M
-41
27.25
(f
-54
II
«
-34
28
•«
-50.5
19
HaO«.3|H/)
-24
29.9
M
-45
20
l(
— 17.801
•«*-33-3
M
-42.3
21
M
-21.5
36
M
-41.4
22.22
(i
— 23.6
36-5
" +Hao«.Hyo
-43
23 -5
f<
-12.S
37
HaO«.HdO
-40.5
22.5
HCI044H^a
1+3
38
M
-39.5
22.75
u
28
40.8
«
-37-6
24
«
40
43-7
«
-375
26
u
5oiB.i>t 50
M
-38.8
27
M
45
59-9
«
-47.8
22.5
ROO^.iBfifi
«7-5
715
«
-44
24
u
17
77.2
U
-43-5
24.5
u
+2.2
833
M
-43-2
25
M
-21.5
90.7
U
-44.5
26
U
-40
94
m
-37-2
25
BCX>^Bfia+BCKk-iiBfi
— loa
100
1"
477 PITBOLBTJM ETHBB
PETROLEUM ETHER.
100 cc. HiO dissolve 0.005 cc- petroleum ether at 15^ (Groadiuff. 19x0.)
PHENACETIN (p Acetphenetidin) C«H4(0C,Hi)NHCH,C0 p.
Solubility in Aqueous Alcohol at 25".
(Seidell, unpublished.)
Cms. Sat. SolutioiL movent. !mt. bol. Gms. Sat. Sokition.
0.0766 70 0.879 6-2S
0.14 80 0.858 7.63
0.28 85 0.847 7-88
0.65 90 0.834 7.82
1.50 92.3 0.827 7-70
2.85 95 0.821 7.45
4.55 100 0.806 6.64
100 gms. H|0 dissolve 1.43 p^ms. phenacetin at^the b. pt. (U.S.P.,vm.)
too gms. 92 .3 wt . % alcohol dissolve about[50 gms. phenacetin at the b. pt. "
Solubility of Phenacetin in Several Solvents.
(SeideU, 1907.)
Gms. Phenaoetta Gms. PhenaoeCiii
Solvent. t*. per 100 Gms. SohreuL t*. per 100 Gms.
Sat. Solution. Sat. Solution.
Acetone 30"3i 10.68 Benzene 30-31 0.65 (0.873)
Amyl Acetate 30-31 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 30-31 946 (1.025) Xylene 32.5 1.25 (0.847)
Benzaldehyde 30-31 8.44 (1.063)
(Figures in parentheses are Sp. Gr. of Sat. Solutions.)
100 CC. petroleum ether dissolve o.oi 5 gm. phenacetin at room temp. (Salkower, 19x6.)
too gms. pyridine dissolve I7'39 gms. phenacetin at 20-^5^. (Dehn,z9t7.)
too gms. aq. 50% pyridine dissolve 28.94 ff^s. phenacetin'at 20-25^ **
Wt. % CH^H
insolvent.
dtfof
SatSoL
0 (water)
10
20
I
0.984
0.968
30
0.952
40
0.93s
so
60
0.917
0.898
PHKNANTHRAQUINONS C«H4CO,CO,CeH4.
SoLUBiLrrY IN Benzene and in Ethyl Acetate
•
OVrer. 1910.)
Solubility in
Benzene. Solubility in Ethyl Acetate.
«•.
Sp. Gr. of
Sat. Solution.
Gms. (CHJ,(CO0i
per IOC Gms. tr.
Benzene.
Sp. Gr. of
Sat. Solution.
Gms.(C|H«)j(CQi)t
per 100 Gms.
Ethyl Acetate.
10
0.8902
0.412 10
0.9102
0.518
IS
0.8850
0.471 20
0.9025
0.626
20
0.8800
0.538 30
0.8906
0.770
30
0.8698
0.738 40
0 . 8789
0.99s
40
0.8601
1.032 SO
0.8674
1.292
SO
0.8506
1.354 60
0.8561
1.640
60
0.8415
1.760 65
0.8508
1.902
70
0.8327
2.687 70
0.8454
2.215
80
0.8241
3 770 7S
0.8401
^'S^S
Note. — The Sp. Gr. determinations given in the above table and in the tables
for anthracene ana anthraquinone, pp. 81 and 82, are not included in the original
paper of Tyrer (iQio) but, in response to my request, have been kindly supplied
lor the present volume. I am also indebted to Ur. Tyrer for the moaifiea form
of his original tables showing the solubilities of anthiaqoinone and phenanthra-
quinone in mixed solvents. (A. SJ
PHENANTHRAQUINONE
478
Solubility of Phenanthraquinonb in Mixturbs of Organic Solvents.
(Tyrer. 1910.)
In CHCU + Pentane In CHiCOOCiHs + Hydro-
carbons(i) at 48®.
Per cent Cms. PI
thnquinone
In C«He + Hydrocarbons
(i) at 48^
Per cent
CAin
Mixed
Solvent
O
10
20
30
40
SO
60
70
So
90
100
Cms. Phenan-
thxaquinone
per xoo Cms.
Solvent.
0.0708
0.088
O.I18
0.160
0.228
0.318
0.440
0.588
0.772
1.004
1.288
Percent
CHCUin
Mixed
Solvent.
O
10
20
30
40
SO
60
70
80
90
100
at i±.S^.
Gni8. Pfaenan"
per xoo Cms.
Solvent.
0.025
0.045
0.080
O.II5
0.165
0.220
0.330
0.525
0.805
1. 415
2.402
CHiCOOCiHt
mMized
Sotveat.
O
14.19
27 -37
39-94
52.12
6356
74.19
84.62
90
100
Cms.
thzaquinone
per xoo Gnu.
Solvent.
0.073
0.126
0.207
0.33s
0.494
0.656
0.817
0.993
1.073
1.230
(x) Distilled from peCioIeum, b. pt. « Sa'-ga*. (See note, preceding page.)
PHENAirrHBEME CuHio.
Solubility in Alcohol and in Toluene.*
(SpeycTB — Am. J. 80.(4] X4t ^95* 'oa.)
In Alcohol. In Toluene.
Cms. Ci4?it per
t*. xoo Grams
CsHftOU.
O 3'^S
10 3.80
20 4.6
«S S'S
30 6.4
40 8.2
50 10.6
60 15.6
70 33 o
80
• Calcolated from the original results which are given in terms of gram moleculet of Phffniifhftne
per xoo gram molecules of solvent, and for irregular intervab 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.
Sp. Gr. of
Solutions
Gms. CiiHit per
Sp. Gr. of
Solutions
100 Grams
CH«Oat4'0
(HjO at ^.)
0.814
23.0
0.925
0.807
30. 0
0.929
0.801
42.0
0-934
0.7P9
50.0
0.939
0.797
58.0
0943
0.795
76.0
0.9SS
0.794
95 0
0.971
0.797
115 0
0.989
0.815
13s 0
1.007
0.865 (76.4°)
iSS-o
1.027
Add.
Acetic Acid
((
((
u
((
Butyric Acid
(( it
23
39
70.5
23
39
Gms. CjaHio
per xoo Gms.
Sat. Sol.
8.31
9.8
34-6
156
21
Add.
Propionic Add
(Timofeiew, 1894.)
Gms. CuHm
t*. per too Gms.
Sat.SoL
ti
u
ii
t(
23
39
62.4
23
39
17
21.4
40.3
12.3
16.6
(Aschan, 19x3.)
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 el, 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 PHENAirrHBEME
Solubility of Phbnamthkbnb in Several Solvents at 25^
(HUdebrand, EUefson and Beebe, 19x7.)
Sohreat. ^^^»^iR^*~ Sohrent. ^^"S^S&l^J**
Alcohol 4.91 Carbon Tetrachloride 26.3
Benzene 59.5 Ether 42.9
Carbon Disulfide 80.3 Hexane 9.15
SOLUBIUTT OF PHBNANTHRENB PiCRATB IN ABSOLUTE AlCOHOL.
(Behioid, Z893.)
Gxams per zoo Gnuns Saturated Sohitioii.
*• c * ^
Piaac Add + Pheoanthxcne * Phenanthrene Picnte.
12.3 0.91 0.71 1.62
14.3 I. 00 0.78 1.78
17.5 1.05 0.82 1.87
Solubility op Phenanthrene Picrate in Alcoho;.ic Solutions
Containing Picric Acid and also I^enanthrbnb.
(Behrend.)
Gxams Added to 6a cc. Aba. Alcohol. Gms. per loo Gms. Sat. Sokitioo.
%; , * ^ , * ^
P. Picrate + Picric Ac. + Phenanthrene. Picric Ac. + Phenanthrene * P. Picrate.
2.3 * 1.4 o 0.5 0.534 1. 413 1.947
2.3 1.4 O 0.9 0.409 2. 141 ^550
a-S o.S o 2.1 0.354 2.77 3124
2.3 0.8 o 4.0 0.139 5.626 5765
7-S x-4 0.1 o 1. 159 0.75 1. 91
7.5 1.4 0.2 o 1-285 0.68 1.97
7.5 1.4 i.o o 2.45 037 2.82
7.5 1.4 4.0 o 6.15 0.195 6.345
7.5 1.4 0.0 2.2 0.423 3276 3.699
PHENOL CJiiOH.
SoLUBiLrrY in Water.
(Alezejew, x886; Scfareinemaker, 1900; Rothmund, 1898.)
The determinations were made by the "Synthetic Method," for which,
Note, p. 16.
Gms. Phenol per xoo Gms.
Aqueous Layer.
Phenol Layer.
10 75
75
20 8.3
72.1
30 8.8
69.8
40 9.6
66.9
SO 12
62.7
S5 14 1
595
60 16.7
55 -4
6s ai.9
49.2
68.3 (crit. temp.)
33 4
Results confirming the above, and also viscosity measurements, are g;iven by
Scarpa (1901).
The complete J" — « data for the system are given by Smits and Maarse (191 1).
F.-pt. data for the system are given by R6zsa (191 1; and Patemo and Ampola
(1897).
Vaubel (1895) states that 100 gms. sat. aqueous solution contain 6.1 gms.
phenol at 20*^. Sp. Gr. of solution » 1.0057.
PHENOL
480
PHENOL.
SOLUBILITT OF PhBNOL IN AqUBOUS AcBTONB SOLUTIONS.
(Schretnenukers, 1900.)
In 4.24%
Acetone.
Gmnf Phenol per
xoo Gms.
In 12.2%
Acetone.
Gms. Phenol per
100 Gms.
In 24.6%
Acetone.
Gms. Phenol
xoo Gms.
20
30
40
SO
60
1:
AfLAoetono
Lajer.
• • •
S.o
5.5
S-7
6.S
9.0
14.0
(84^ 22, s
•^
Phenol
Layer.
Aq./
Acetone
!ftS»
Phenol
Layer.
74.0
4.0
71.0
70.0
• • •
• • •
67.0
S.o
67.0
6x.o
...
• • •
Si.o
7S
S7S
34.0
10. S
49. S
20.4*
30. s*
(90.3**)
25.
0
Aq. Acetone
LaTcr.
• • •
6.0
• • •
8.0
Phenol
Layer.
a . •
• • •
64.0
t85<
19.0 57.0
14.0 52.5
23. of 47- of
26. 5I 44- ot
(90. 5"*) 3S. o
In 59.9%
Acetone.
Gms. Phenol per
loo Gms.
Aq. Acetone Phenol
Layer.
26.0
28.5
32.0
34. 5}
(49-5) 41.S
60.5
57.0
52.0
49- of
46.5!
I47*.S
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^
m
Results at So*.
Gms. per xoo Gms. Mixture.
Gms. per 100 Gms. Mixture.
Gms. p
B<0.
er 100 Gms. Mixttnc
HA
(CH^tCO.
CAOH.
H/).
(rH,),co.
CiHdOH.
(CH^tCO.
CAOH.
92
0
8
18.4
34-1
47 S
83 -3
3-7
13
92.3
1-7
6
17.2
25-8
57
82
9
71
10
91
4
S
17.9
81. 1
64
74
•7
.13.8
"S
88.4
7.6
4
19. 1
13.9
68
61
.8
20.2
18
81
IS
4
21. 1
9 9
69
52
5
245
23
70.9
231
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
SI. 6
34-9
13. S
27.1
2-3
70.6
33
4
156
SI
39.8
40.2
20
28.7
1-3
70
35
4
II. 6
S3
28.9
431
28
30
o-S
69s
40.
S
7-5
52
21.8
40.2
38
•
49
62
7
■7
4-3
2.8
46
34 S
SOLUBILITT OF PhBNOL IN BSNZBNB AND IN PARAFFIN.
(Schweissinger, 1884-85.)
Solvent.
Paraffin
Benzene
Gms. QHiOH per too Gms. Solvent at:
16:
1.66
2.S
ax"
8.33
as*.
10
43'.
5
ICO
Data for equilibrium in systems composed of phenol, water and each of the fol*
lowing compounds are given by Timmermans (1907): NaCl, KCl, KBr, KNOt,
K1SO4, MgSOii» tartaric add, salicylic add, succinic add and sodium oleate.
48i
PHENOL
MisciBiLiTT 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.
/ * s
oc Aq. KOH. cc. Aq. Insol. Cmpd. Gms. Phenol.
S 2 (= 1.64 gms.) Octyl * Alcohol 2.6
S S (= 4.1 gms.) "
S 2 (= 1.74 gms.) Toluene
5 3 (= 2.61 gms.) Toluene
5 2 (= 1.36 gms.) Heptane
u
3-9
4.9
6.7
IS
* "i the noimal secondazy octyl alcohol, i. «., the so-called capryl alcohol, CH«(CH«)|.CH(OH)C^
Solubility of Phenol in Aqueous Solutions of Dextro Tartaric
Acid and of Racemic Acid.
(Schreinemakers, 1900.)
In 5.093% Acid.
In 19.34% Add.
[n 40.9% Add.
Gms. Phenol per
xooGflu.
Gms. Phenol per 100 Gms.
Gms. Phenol per loo Gnu
f.
Aq. Acid
Phenol
t*.
r »
Aq. Acid Phenol
Layer. Layer.
f.
'Aq. Add. Phenof
Layer. Layer.
Layer.
Layer.
30
7-5
725
so
10 77
70
13
so
10. s
65 s
60
12. S 72
80
16. S 77
60
I4S
S8
70
19 64
8s
20 74
6S
19s
S3
".
29 56
90
26.5 71
67.
S 25
48s
77*
47
^K
39 63. s
69*
475
97*
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 aj ao^r
(Herz and Fischer — Ber. 37i 4747. '04.) (Vaubel— J. pr. Ch. {2] 67# 476» 'op
Millimols Phenol
per xo cc.
Alcoholic Aqueous
Layer. Layer.
0-7S
0.9
I.I
Q.6
54- 1
0.047
0.05
0.07
o. 16
3.83
3-9
Cms. Phenol
per xoo cc.
< * >
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
Volumes of Solvents
used per
I Gm. Phenol
Gms. Phenol in;
QA
HsO
Layer.
5occ.HjO+ 5occ.CeHe o. a86 0.714
o. X188 0.82x2
0.0893 0.9107
0.0893 a 9x07
u
M
+ XOO cc.
+ x5bcc ••
<f 2000c.
cc
Distribution of Phenol between Water and Benzene at 20**.
(Philip and Bramley, xgxs-)
Gms. Phenol per Liter.
Aq. Layer, a. CcH« Layer, 6.
0.94s
0.888
O.71I
OS94
0-47S
2.073
1.944
I 553
1.293
I 036
Ratio-*
a
2.194
2.189
2.184
2.176
2. 181
Gms. Phenol per Liter.
/ -» V
Aq. Layer, a. C«H« Layer, 6.
0.356
0.238
O.II9
0.0601
0.7736
0.5177
0.2594
O.I314
Ratio-.
a
2.173
2.17s
2.180
2.189
^ Results are also given for the effect of NaCl, KCl and of LiCl upon the above
distribution.
PHENOL
482
Distribution op Phenol between Water and Benzene and
BETWEEN Aqueous KjS04 Solutions and Benzene at 25**.
(RoUunund axid WilBmora— >Z. phyaik. Ch. 40^ 633, 'oaO
Note. — The original restdts, which are given in terms of gram
mols. per liter, were calculated to grams per liter, and plotted on cross-
section paper. The following figures were read from the curves
obtained.
Between B
aOaiidC«Ht.
CtHiOH
Effect of KsSOi upon the DistribntioD.
Grams
Gnu. KsS04
(2) Gms.
CeHfOH
iter of:
0)Gm8. CaHsOH
per Liter of:
per Liter
Aq.
perU
Aq.
per Liter of:
6sO
^CeH^
Aq.
^CeHe
Ligrer.
Layer.
OOlUuuu.
Layer.
Layer.
Layer.
Layer.
5
10
1.36
17.08
59 96
952
26.28
10
28
2.72
16.92
60.63
9 50
26.38
IS
52
5-44
16.85
60.92
9.46
26.5s
30
84
10.89
16.44
62.73
9-35
27.06
«s
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
SO
520
610
(z) First aeiiet.
(a) Second series.
Equilibrium in the System Phenol, Benzene and Water at 25**.
(Horiba, 1914-1916.)
, Gms. per zoo Gms. Sat. Sol.
t
QHiOH.
CA.
H.O.''
Solid Phase.
81.06
18.94
0
CH^H
89.78
7.92
2.30
M
92.31
4.07
3.62
W
95-14
0
4.86
M
esults for the conjugated liquid layers are as
follows:
•
Upper I^yer
•
Lower Layer
.
Gms. per 100 Gms. of the Liquid.
Gms. per 100 Gms. of th<
/ «-
C,H,0H. CH,.
t Liquid.
CiHiQH.
C.H,.
H^.
H,0.
0
99-95
0.05
0
0.198
99.803
4.78
94.98
0.24
1-43
0.21
98
36
17.36
81.83
0.81
2.80
0.21
96
99
21.15
77.22
1.63
3.01
0.21
96
•77
28.01
69.81
2.18
3-35
0.21
96
44
44.39
50.56
505
4.07
0.19
95
74
SS.80
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.
80s
Data for this system are also given by R6zsa (191 1).
The coefficient of distribution of phenol between olive oil and water at 25**,
cone, in oil + cone, in HtO, 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
ghenol in olive oil by the solubility in water, each being determined separately.
Lesults 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".
483
PHENOL
Distribution op Phenol between Water and Carbon Tetra
Chloride at 20°.
(Vaubel— J. pr. Ch. (aj 67, 476, '03)
Gms. Phenol
Uied.
Volumes of SblTents.
GramB Phenol in:
I
I
I
I
I
Z
I
50 cc. H,0+ 10 cc. CCI4
+ 20 cc.
+ 30 cc.
+ so cc.
+ 100 cc.
+ 150 cc.
+200 cc.
u
ti
ti
ti
it
u
(I
tt
«
14
HsO Layer.
0.8605
0.7990
0.727s
0.643s
0.4680
0.3645
0.3240
CCI4 Layer.
0.1285
0.1900
0.2615
0-34SS
0.5210
0.6245
0.6650
Distribution of Phenol between Water and Organic Solvents at 25^
(Hen and Rathmann, 19x3.)
Results for:
HsO and Chloroform.
Mols. CAOH per Liter.
HtO and Carbon
Tetrachloride.
Mols. C»H»OH per Liter.
HtO and Tetrachlor
Ethane.
Mob. CAOH per Liter.
HfO Layer.
0.0737
0.163
0.2II
0.330
0.436
CHCl, Uyer.
0.254
0.761
1.27
3 36
S-43
HtO Layer.
0.0605
0.140
0.213
0.355
0.489
0.525
CCI4 Layer.
0.0247
0.072;
O.I41
0.392
1-47
2.49
HtO Layer. CiHt CI4 Layer.
0.023
0.0345
0.081
O.II4
O.151
O.IS5
0.061
0.094
0.265
0.406
0.617
0.651
HiO and Pentachlor
Ethane.
Mols. C«H|0H per Liter.
H,0 and Trichlor
Ethylene.
Mols. C«H,OH per Liter.
HsO and Tetrachlor
Ethylene.
Mols. C«H|0H per Liter.
H,0 Layer.
0.0420
0.0866
0.150
0.222
0.280
0.333
CiHCU Layer.
0.0495
O.IIO
0.226
0.432
0.708
1. 170
H/) Layer. CHC1:CC1| Layer. H,0 Layer. CCI«:CC1| Layer.
0.044
O.IOI
0.180
0.236
0.277
0.339
0.046
0.107
0.236
0.388
0.55s
0.986
0.0653
0.143
0.327
0.421
0.490
0.0277
0.0650
0.198
O.4II
0.684
Distribution op Phenol at 25° between:
(Hers and Fischer — Ber. 38, Z143, '05.)
Water and Toluene.
Water and m Xylene.
Minimols CeHsOH
per 10 cc.
Layer.
Grams CeHsOH
per 100 cc.
Millimols CeHsOH
per 10 cc.
Grams CeHsOH
per xoo cc
C^HiCB^
Layer.
1.244
3 047
4.667
6.446
14.960
17-725
47 003
53-783
90.287
0.724
1.469
2.200
2.861
4.750
5 346
7.706
8.087
9.651
CeHsCHs
Layer.
1. 169
2.865
4.389
6.061
14.07
16.69
44.20
50.58
84.89
Layer.
0.681
1. 381
2.068
2.691
4.467
5.027
7.246
7.604
9.074
ffi'
CiH4(CH,),
Layer.
1. 610
4.787
12.210
22.718
34827
51-352
77-703
HsO
Layer.
1. 071
2.726
5.168
6.994
8.124
9,123
10.050
Layer.
i-SU
4.501
ri.22
21.36
32.75
48.28
73 07
HtO
Layer.
1.007
2.563
4.860
6.577
7.64c
8-57^
9-4SC
PHKNOL 484
Freezing-point Data (Solubilities, see footnote, p. i) Are Given for
Mixtures of Phenol and Each of the Following Compounds:
Dimethylpyrone. (Kendall, 1914a) Bromotoluene. (Paterno and Ampola, 1897.7
Phenylhydrazine. (Cuisa and Bemaidi, 19x0.) 0 Toluidine. (Kremann. 1906.)
Picric Acid. (Philip, 1903; Kiemann, 1904.) t Toluidine. (Kxcmann, 1906; Philip, 1903.)
Picric Acid +Other Cm'p'ds. (Kremann, '04.) Urea (Kremann ft Rodenis, 1906; Philip, 1903.)
Pyridine. (Bramley, 19x6; Hatcher ft Skiirow,i9i7.) Methyl Urea. (Kiemaxm, 19x0.)
Quinoline. (Braml^, 1916.) as Dimethyl Urea. "
Kesorcinol. (jaeger. 1907.) f Dimethyl Urea. "
Sulfuric Acid. (Kendall and Carpenter, 1914-) Urethan. (Mascardli ft Pestakssa, 1908, 1909.)
Thymol. (Pateroo and Ampola, 1897.) P Xylene. (Patexno and Ampola, 1897.)
m Xylidene. (Kranann, 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:
Cms. Phenolate per zoo Gms. Gms. Phenolate per 100 Gms.
f. t • s
Aq. Layer. Phenolate Layer.
IIO 9 76
120 12 69
130 17 S 60 .
140 crit. temp. 40
AminoPHENOLS. See last line p. 138.
^ TribromoPHENOL CeHsBriOH.
Data for the solubility of mixtures of symmetrical tribromophenol and symmetri-
cal trichlorophenol in diluted methyl alcohol at 25° are given by KQster and Wiirfel
(1904-05). The results are presented in terms which are not dearly explained.
Solubility of Mixtures of s Tribromo Phenol and s Trichloro Phen(h«
IN Methyl Alcohol at 25^
(Thiel, X903; from WOrfel, 1896.)
Molecular per cent C«Ht.OH.Bri n Solubility of „ ,
• .
Aq. Layer.
Phenolate Layer.
10
3
94
30
4
93
so
s
91
70
6
87 s
90
7
83
InSotid.
In Solution. '
CfHs.OH.Cls.
C6Ha.OH3i».
xuiau
0
0
0.204
0
0.204
4.49 ■
3 59
0194
0.007
0.201
10.13
7-58
O.19I
0.016
0.206
16.28
12.15
0.172
0.024
0.196
62.44
13 07
0.204
0.031
0235
69.88
IS 86
0.150
0.028
0.178
81.76
19.01
0.096
0.023
O.I18
84.66
24 OS
0.069
0.022
0.091
87 53
32.46
0.043
0.021
0.063
93.62
47.87
0.021
0.019
0.040
100. 0
100. 0
CO
O.OZ9
0.019
NitroPHENOLS CeH4(OH)NOs 0, m and ^
i(X) gms. sat. solution in water contain 0.208 gm. 0 nitrophenol at 20^.
^* " " " 2.14 gms. m
" " " 1.32 " p " " (Vaubd,x89S.)
F.-pt. data for mixtures of m nitrophenol and water and for p nitrophenol and
water are given by Bogojawlewsky, Winogradow, and Bogolubow (1906).
485
NitroPHENOLS
C6H4(OH).NOi 0, m and p.
Solubility of Each Separately in Water. (Sidgwick, SpuneD and Davies, zgxsO
f.
Cms. per
100 Gms. Sat. Sol.
*•
Gms. per 100 Cms. Sat. SoL
Ortho.
MeU.
Paxa.
• .
Ortho. Meta. Paxa.
40
0.330*
3.02*
3.28
100
1.078
50
0.388
3.68
4.22
no
1.37
60
0.463
4.54
5.53
120
1. 59
70
0.560
5.80
750
120
1. 91
80
0.68s
7.90
10.85
140
2.32
90
0.856
11.69
21.2
ISO
2.90
92.8
crit. t. ...
• • •
00
160
3. 75
98.7
crit. t. ...
00
• « •
200+
crit. t 00
* in above table indicates that a solid phase is present.
The above determinations were made by the synthetic method. M. pt. of 0 »
44.9**; of f» = 95.I^ of ^ = 113.8®. Triple pt. for 0 = 43.5® at cone. 99.^8 and
0.35; for tn = 41.5® at cone. 74 and 3.16; for p = 39.6® at cone. 71.2 ana 3.26.
One liter sat; solution in water contains 3.89 ems. o nitrophenol at 48**.
One liter sat. solution*in 1,0 n 0 C«H4(0Na)N0i contains 9.6 gms. 0 nitrophenol
at48^ " (Sidgwick.'xo.)
Solubility of o Nitrophenol in Liquid Carbon Dioxide. (Badmer. 1905-60
Gms. < C«H,a)H)NOi
per 100 Gms.
f.
Sat. Sol.
-52
1.9
-40
2-5
— 20
3-8
0
S-2
+10
7-7
Gms. 0 C|H4(pH)NQi
per xoo Gms.
t*.
Sat.Sol.
".5
10
14
21.2
15
33.8
16
48.5
20
60.7
100 gms. 95% formicacid dissolve 16.06 gms. oC«H4(OH)NOt at 20.8®. (Aichaii, 'xj.)
100 gms. 95% formic acid dissolve 23.44 gms. p CeH4(OH) NOi at 1 8.6'. "
One liter of sat. solution of the pale yellow form of p nitrophenol in benzene*
contains 7.1 gms. p CeH4(0H)N(S at 5*, determined by the t.-pt. method.
(Sidgwkk, X9X5.)
Solubility of the Three Nitrofhenols, Separately, in Toluene,
BroMOBENZENE and in Ethylene DiBROMIDE. (Sidgwick, Spurrdl and Davies, 1915.)
Gms. 0 CJI«(0H)N0| per xoo Gms. Sat. Sol
Gms. ^ C|H((OH)NO| per loo Gms.Sat. SoL
*• *
' inCHiCHi. InCiHtBr.
In CtHiBr,.
[n QHtCHa. In CABr. InCtHiBrt.^
»S
46.9 • • •
40
70
18. 5
31
30
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
lOO
79.6
80.6 88.5
35
84.5 78.3
79
no
96.3
96.3 98
40
93.1 89.7
90.6
Gms. M C|H4(0H)N0|
Gms.
mC.H«(0H)N0i
Gms. M QH«(OH)NOb
f.
per xoo Gms. Sat. SoL
t*. per xoo Gms. Sat.
Sol. V.
per xoo Gms. Sat. S6L
in C|H|CH|.
inCACHt.
inCACHi.
39-6
4.63
64.8
16.44
78.5
70.50
45-8
6
67.7
20.26
82.3
79.57
48.9
7 03
715
33-^^
88.8
91 -43
54
9. II
74-5
46.93
95-1
XOO
58
11.28
75-7
57.71
DiNitro PHENOL C6H<.0H.(N0,)>.
ICO gms. abs. methyl alcohol dissolve 6.3 gms. C6Ht.0H.(N0s)s at 19.5^.
100 gms. abs. ethyl alcohol dissolve 3.9 gms. CsH«.OH. (NOi)i at 19.5^. (deBmyn, '9^^
PHENOLS
486
«•
««
11
11
41
41
II
II
Frbbzing-point Data (Solubility, see footnote, p. i) Akb Givbn fob thb
Following Mixtures Containing Substituted Phenols.
0 Bromophenol + p Bromophenol. (HoUemn and Rinkcs, 1911J
0 Chlorophenol + ^ Chlorophenol.
0 lodophenol + P lodophenol.
5 Tribromophenol + 5 TrichlorophenoL
2.4.6 Tribromophenol + Acetyl tribromophenol.
0 Chlorophenol + Quinoline.
'^ 4- Pyridine.
0 Nitrophenol + Acetyl 0 Nitrophenol.
0 Nitrophenol + a Dinitrophenol.
^r P Toluidine.
P Nitrophenol + P Nitrosophenol.
Each of 0» m and p Nitrophenol + Dimethylpyrone.
^' + Picric Acid.
-|- Sulfuric Acid.
+ Urea.
2.4 Dinitrophenol + Dimethylpyrone.
PHENOLPHTHALEIN (C«H«OH)sCO.CeH4CO.
ioogms.HsO dissolve 0.0175 iT^- phenolphthalein at 20^.
(Acree and Slagle, 1909.)
" " 0.04 " " at 20-25*. (Delm.»iyJ
Pyridine " 796. gms.
aq. 50% pyridine " 300
PHENYL ALANINE a CeH.NHCH(CHs)COOH.
Data for the solubility of phenyl alanine in aqueous salt solutions at 20^ are
given by WUrgler (1914) and Pfeiffer and Wfirgler (1916).
PHENYLENE DIAMINES 0. m, and ^ C<H4(NHs)t.
Solubility in Water at 20®. (Vaubd, 1895.)
100 cc. sat. solution contain 23.8 gms. m^CcHiCNHOii ^ of sat. sol. « 1.0317.
100 cc. sat. solution contain 3.7 gms. p C«H4(NHs)t» ^ of sat. sol. «« 1.0038.
Ratio of Distribution between Water and Benzene at 25^
(Farmer and Warth, 1904.)
(KOster and Wflrfel. 1904-05.)
(Boeseken, i9xa<)
(Bcainky, 1916.)
fi
(Boeseken, 191 s.)
(Crompton and Whitely, X895O
(Pawlewski, 1893; Philip, 1903.)
(Jaeger, 1908.)
(Kendall, x9X4a.)
(Kremann and Rodeois, 1906.)
(Kendall and (Carpenter, 19x4.)
(Kremann and Rodenis, X906.)
(Kendall, X9i4a.)
II
II
II
Results for m Phenylene Diamine.
rt .. oonc. C|H(i
Ratio ^=?«
0.182
0.176
Gms. m CtH4(NH«)s per:
, * ,
50 cc. C«H«. 1000 cc. H^O.
0.0828 9.088
0.0463 5.260
Solid Phase.
f.
Results for 0 Phenylene Diamine.
Gms^o^(NH|), per: cone. CH,
i * ■ \ Ratio jj-^»
so cc. C«H«. 1000 cc. H|0. ^^^ "«^
0.0273 0.9818 0.556
0.2040 7 5470 0.541
PHENYL HYDRAZINE CHsNH.NH,.
Reciprocal Solubility op Phbnylhydrazine and Water, Detbrminbo
BY THE Freezing-point Method. (Biankama, i9xa)
Gms.
^^gS Solid Phu..
Sat. Sol.
Ice 19.8 60 . 1 C|EUNHJra..iHdO
20.4
21.8
+(^ANH.NHi.iH|0 23
+ I 4.7 CiHjrajra,.jH/) 24.2
26.1
26.2
2S-7
23.2
17
16.6
19.6 m. pt. 100
Between the concentrations 10.9 and 60.1, two liquid layers are formed. See
p. 487.
Gms.
«. r,H|NU.NRi
per loo Gms.
Sst.SoL
0
0 I
03
2.3
0.6
3-9 '
0.7
4.6 •
I
7
4-7
6
II. 6
7
15
16.8
8
9.6
19.6
10.9
if
f(
«
II
II
II
II
II
64.2
75
79.2
837
91
92.3
93-7
97.2
98.8
99
ti
II
II
II
II
If
II
(I
+CANH.NH^
CANH.NH|
487 PHENYL HYDRAZINE
Rbciprocax* Solubility of Phenyl Hydrazine and Water. (Con.)
The temperatures of sej^ration into two liquid layers of mixtures containing
from 10.9 to 60 per cent QHtNH.NHs, are:
t»^f Cms. CANH.NHs ^^r Cms. CANH.NH« ^. . Cms. CANH.KH1
S«P*»*»»»- ^lixture. Separation. Mixture. S>ci»nition. 'Mixture.
19.8 II. 6 54. 6 29.7 50.6 48.9
34 138 SS'^ 31-4 SO Si-2
45 i^S SS.2crit. t. 33.6 46 53.5
49.4 18.7 sS-2 369 44.2 54.7
52.4 21.9 S5 39-3 39-6 56.7
54 25.2 54 41.7 24 59.5
54.4 28.3 52.6 46 19.8 60.1
Additional data for concentrations of CeHsNH.NHi above 60 per cent, are given
by Oddo (1913)-
Benzoyl PHENYL HYDRAZINE C«HtNH.NHC7H»0.
Solubility in Aqueous Alcohol at 25*.
(Holtonun and Antusch, 1894.)
Vol.% ^^??^^ Sp.Gr. Vol.% ^^'^^^f^ Sp.Gr.
Alcoha. J^JStf Sofution.. Alcohol. I^^«- SoTutions.
ICO 2.39 0.793 ^ 1-59 0-859
95 2.43 0.814 70 1.08 0.884
93 3 0.822 SS 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.
Phthalyl PHENYL HYDRAZIDE C6H4< >N.N<
CO CH
Phthalyl PHENYL Methyl HYDRAZIDE C«H4<[ >N.N<
CO CaHf.
Very careful determinations of the solubilities of the enantrotropic forms of
these two compounds in alcohol, chloroform, ethyl acetate, acetone, benzene and
in methyl alconol are given by Chattaway and Lambert (1915). See also p. 312.
Acetone PHENYL HYDRAZONE (CH«)sC.NsHCtH5.
Data for the System Acetone Phenyl Hydrazone + Water Are Given
BY Blanksma (1912).
The following results were obtained for the solubility of (CHs)sC.Nt.HC6H<.HtO
in water.
f.
Gm8.(CHi)sC.N,.HC«H|
pet 100 cc. Solution.
Solid Phaae.
0
0.090
(CHi)iC.N« HCA-H«0
IS
0.187
M
32.8
0.412
If
DibromoPHENYL SELENIDE and TELLURIDE (C6H6)sSeBrs,(CeH»)sTeBrs.
Data for the solubility of mixtures of dibromophenyl selenide and dibromo-
phenyl telludde in benzene at 21^ are given by Pellini (1906).
PHLOROCFLTTCINOL 1.2.3 'C«Ha(0H)j.2H,0.
100 gms. HiO dissolve i .13 gms. phloroglucinol at 20-25®. (Behn, '17.)
^' pyridine " 296
" aq. 50% pyridine " 134
FHOSFHO MOLYBDIC ACID 488
PH08PH0 MOLYBDIC ACID PiO».2oMoO|.52HsO.
Solubility in Ether. (Parmentier, 1887.)
t*. o'. 8.i'. x9j'. a7.4'. stjgr.
Gms. Add per 100 gms. Ether 80.6 84.7 96.7 103.9 107.9
PHOSPHORUS P. (yellow)
Solubility in Benzbnb.
(Chxistomanos — Z. aiuvg. Ch. 45. 136, y>5.)
«o Gms. P per Sp. Gr. of ^e Gms. P do- Sp. Gr. of ^.e Gms. P per
^ * xooGms.CeHc. Solution. * ' too Gms. CA- Solution. * * xooGms.C^
o 1. 513 ... 23 3.399 0.887s SO 6.80
S 1-99 ••• 2S 370 0.8861 ss 7-3^
8 a. 31 0.8990 30 4.60 ... 60 7.90
10 2.4 0.8985 35 S17 ••• ^S S-40
IS 2.7 0.894 40 S-7S ••• 70 890
18 3.1 0.892 4S 6. II ... 7S 940
20 .3.2 0.890 81 10.03
Solubility op Phosphorus in Ether.
(Chxistomanos.)
Gms. P per «,» r* «* Oms. P per «_ o, «f Gms. :P per
(CrfljOsO. Sdutiflos. (CA)aO. Solutions. (CsHi)sO.
o 0.434 ... 15 0.90 0.723 28 1.60
5 0.62 ... 18 I. 01 0.719 30 1.7s
8 0.79 0.732 20 1.04 0.718 33 1.80
zo 0.85 0.729 23 1. 12 0.722 35 2.00
25 1-39 0.728
Solubility of Yellow Phosphorus in Several Solvents at I5^
(Stich, X903.)
Solvent. ^^ISSiiS?^^
Almond Oil 1.2s
Oleic Acid 1.06
Paraffin 1.45
Water 0.0003
Acetic Acid (96%) o . los
Solubility of Phosphorus in Carbon Disulfidb.
(Cohn and Inouye, i9r>.)
Gms. P Gms. P Gms. P
If. per 100 Gms. C*. per 100 Gms. t*. per 100 Gms.
Sat. SoL * Sat. SoL Sat. Sol.
— 10 31.40 ~3S 66.14 o 81.27
-7-S 35-85 -3-2 7172 +5 86.3
-5 41.95 -2.5 75 10 89.8
The above determinations were made with very great care. The authors show
that the previous determinations of Giran (1903) are inaccurate.
1 00 gms. alcohol (i= 0.799) dissolve 0.31 2 gm. P|Cold,ando.4i6gm.,hot.(Bac]mer)
1 00 gms. glycerol (<iij = 1.256) dissolve 0.25 gms. Pat 15-16®. (Ossendowski* 1907.)
Red phosphorus is completelv 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. (Colsoa, X907.)
489 PHOSPHORUS
RBapROCAL Solubility op Phosphorus and Sulpur, Dbtbrminbd by
THB Synthetic (Sealed Tube) Method.
(Ginn, 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 ciui^es.)
Eutectics.
M
[axima of Cm
rves.
f.
Mob. % S in
Mixture.
SalidPliaae.
V.
Mob.%Si]i
Mixture.
Solid Phase.
-40
33 S
P4S,+P,
+167
43-6
PiS.
+46
SO
P4S,+PA
296
60.8
PA
230
67. S
P|S,+P,S,
272
72.1
PfS.
243
75
P«S,+PS,
314
86.1
PS.
Additional data for this system are given by Boulouch (1902 and 1906) and by
Helff, 1893.
PHOSPHORUS ST7LFIDE8 P4S,, P4S7, P4S10.
Solubility in Carbon Disulfide, Benzene, and in Toluene.
(Stock, 1910.)
" ^ xoo
f.
Gms. PiS| per zoo
Gms.:
Gn8. P4Srger 100
Gms. CS|.
Gfflft. PiSiope
CS,.
CA-
Gms-CSi
— 20
II. I
• mm
...
...
0.083
0
27
• • •
...
0.005
0.182
+17
100
2-5
3 "5
0.0286
0.223
80
• ■ •
II. I
• • •
• . •
• • •
IIO
• • •
■ • •
lS-4
• • •
• • •
PHOSPHOBIC ACID (ortho) HsPOi.
Solubility in Water. (Smith and Meiukimsog.)
(The sat. solutions were analyzed by titration. The mixtures were constantly
stirred for at least two hours.)
f.
per 100 Gms.
Solid Phase.
f.
Gms. iU*0|
per 100 Gms.
SoUdPlius.
Sat.SoL
Sat. Sol.
-8i*
62.9
Ice+2HtP04.H^
24.38
94.80
ioH^POi.EW)
-16.3
76.7
iBJfOtSfi
24.40
94-84
U
+ 0.5
78.7
ft
24.81
94.95
m
14 -95
81.7
«<
25.41
95.26
u
24.03
85.7
(1
25.85
26.2*
95.54
i«
27
87.7
II
• • •
«f
+HyPQ,
29 iS^
90. s
w
26.23
95-90
HgPO,
29 -351
91.6
M
27.02
95 98
t
28.5
92. s
M
29.42
96.15
m
27
93-4
W
29.77
96.11
u
25 -4
94.1
l«
37-65
97.80
*
u
23 5*
• • •
l«
+zoH^4-H«0
39-35
98.48
M
34.11
94.78
zoH|P0«.H^
* Eutec.
42.30T
t M.i
100
pt.
W
Note. — The results of Giran (1908), determined by the freezing-point method,
are shown to be erroneous, due to supercooling which would result n^om failure to
induce crystallization by inoculation.
F.-pt. data for mixtures of phosphoric and phosphorus adds are given by Rosen-
heim, Stadler and Jakobsohn (1906).
PHOSPHORIC ACID 490
PyroPHOSPHOBIC ACID H4P«07.
SCM.UBILITY IN Watbr. (Ginn, 1908; see note on pnoedmg page.)
r.
Gms. H4PA per 100
Cms. Skt. Sol.
Solid Phase.
-75
59
IM +H«PA.xiH«Q
+26 m. pt.
86.8
H4PA.iJH^
23
88.8
+H4PA
61 m. pt.
100
H4PA
HypoPHOSPHOBIC ACID H.POs.HsO.
100 ems. sat. solution in water contain 81.8 gms. HiPOi at the m. pt., 62**, of
the hydrated compound, HiPOt.HiO. (Rosenheim and Pritxe, 1908.)
PHTHAUC ACIDS C<H4(C00H)t, 0, m and p.
SOLUBILITT OF EaCH IN WaTER. (Vaubel, 1895. 1899)
Acid. t*. Gms. per xoo Gnu. Solution.
0 Phthalic Acid 14 o . 54
m = Isophthalic Add 25 0.013
p ^ Terephthalic Acid . . . almost insoluble
Melting Temperatures of Mixtures of 0 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 0 Phthalic Acid in Alcohol and in Ether at 15^.
(Bouigoin, 1878.)
Gms. C«H4(C00H)i 0 per xoo Gms.
Solvent. r * \
Solution. Solvent.
Absolute Alcohol 9156 11.70
90 per cent Alcohol 10 . 478 10 . 08
Ether . 0.679 0.684
Solubility of 0 Phthalic Aero in Alcohols. (Timofeiew. 2894.)
Gms. 0 Gms. o
Sat. Sol. Sat. Sol.
Methyl Alcohol — 2 1 5 . i Ethyl Alcohol 21.4 1 1 . 65
" " +19 19.5 Propyl Alcohol — 3 3.42
+21.4 20.4 " " +19 5.27
Ethyl Alcohol - 2 8.2 " " 22 5.54
-I-I9 II 23 5.70
Distribution of 0 Phthalic Aero and of m Phthalic Aero (Isophthalic)
between Water and Ether at 25**. (Chandler, 1908.)
Results for 0 Phthalic Acid. Results for m Phthalic Acid.
Mob. 0 Cai4(C(X)H)i Ratio for Mols. m dH4(C(X)H), Ratio for
per Liter: j^Jt^, Union- P^^I^' RatioJ. Unjon-
H«0 Layer, 0. Ether Layer, ft. Acid. H/) Layer, a. Ether Layer, ft. Add.
0.0261 0.0322 0.809. 0.637 0.000398 0.0485 0.0821 0.0359
0.0x31 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 1.006 0.635 0.000252 0.0266 0.0949 0.0341
Ratio of solubilities of Phthalic acids in olive oil and water at 25^
(Bdeseken and Watennan, 1911, 19x2.)
0 Phthalic acid, solubility in oil 4- solubility in HsO » 0.0 1.
p Phthalic acid (Terephthalic), solubility in oil + solubility in H»0 =■ 9.52.
100 gms. 95% formic acid dissolve 0.55 gm. p phthalic acid (Terephthalic) at
20.2^. CAschan, 19x3.)
491 PHTHAUC ACIDS
NitroPHTHAUC ACIDS oandm(Iso) C«H,(NO,)(COOH)s.
Solubility of the Several Nitro Phthalic Acids ik Water at 25^.
(HoUenum and Httiainga, 1908.)
Acid.
M. pt.
Cms. Add
per 100 Gms.
Sat. Solution.
a Nitro Ortho Phthalic Acid
0 it tt tt ti
Symmetrical Nitro Iso Phthalic Add (anhy.)
u
tt
Asymmetrical
Vicinal ''
tt
tt
tt
tt
tt
tt
220 2.048
164-166 very soluble
255-256 0.220
(hydrated) 255-256 0.157
245 0.967
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.
PHTHAUC ANHTDBIDE C«H«<^3>^-
Solubility in Water.
(van der Stadt, 2902.)
All determinations, except first three, made by the Synthetic Method. See
P- 16. . _
f.
Gms. CAOi
Wat-«r.
per xooGms.
Solution.
Mol. per cent
C.HA.
f.
Gms. Ca
100
BWiPer
Gms
MoL
percent
C.H4O,.
Water.
Solution.
0
0.00295
0.00295
0.00036
189.5
1076
91.66
56.73
25
0.6194
0.6150
0.0754
188.8
1265
92.68
60.63
so
1.630
1.604
0.198
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
3193
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
131
83010
99.86
99.02
191
821.5
89.19
50
131. 2
00
100
100
190.4
863.4
89.62
51-24
Solubility of Phthalic Anhydride in Carbon Disulfide.
(Arctowaki, 1895; Etard, 1894.)
f.
— 112.5
-93
-77.5
-40
— 20
— 10
o
Gms. C«H|0|
per xoo Gms.
Solution.
0.013
0.013
0.016
0.03
0.06
O.IO
0.20
f.
+ 10
20
30
40
50
60
Gms.C|HA
per xoo Gms.
Solution.
0.3
0.7
0.8
1.2
1-3
1-7
Gms. CbHA
C*. per xoo Gms.
Solution.
70 2.3
90 3-7
100 s
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, 19x3.)
100 gms. pyridine dissolve 83.5 gms. phthalic anhydride at 20-25^. (Dehn, 19x7.)
PHTHALIMIDE 492
PHTHALDODE 0 C<H4 < (CO)t > NH.
100 gms. HiO dissolve 0.06 gm. phthalimide at 20-25^ (Ddm, 1917.)
^* pyridine " 14.15 gms.
" aq. 50% pyridine " 774 "
PHTHALONIC ACID COOH.QH4.CO.COOH.2HsO.
100 gms. sat. solution in water contain~64.4 gms. anhydrous acid at 15", Sp. Gr.
of sat. solution » 1*243. CTcfainiijac 1916.)
Amide of PHTHALIDECABB0Z7LIC ACID C«H4<^9(^^^"*^>0 (m. pt.
185.5"). . ^"
100 gms. HsO dissolve 0.132 gm. of the acid at 16.2^ and 5.7 gms. at b. pt.
CTchemiac, 19x6.)
PHYSOSTiaMINS (Eserine) C,»HuN,Oi.
Water dissolves only traces of physostigmine. 100 ems. of a solvent composed
of 3 gms. HtBOt per 100 cc. of aq. 50% glycerol dissolve 2.5 gms. Ci»HuN]Ot at
room temp. (Buoni and BoiUnetto, 191 x.)
PHYSOSTIQMINS SALICYLATE C<H«(OH)COOH.Ci.HuNsOk and Physo-
stigmine Sulfate HiS04(Ci»HsiNsOi)s.
Solubility of Each in Water, Alcohol, etc.
(u. s. p. VUI.)
^ Gms. per 100 Gms. Solvent.
Sohreat. ""
Water
Water
Alcohol
Alcohol
Chloroform
Ether
Methylphenyl PICRAMIDES.
Solubility in Ethyl Alcohol at 18®.
(Hantrach, 19x1.)
100 cc. CsH»OH dissolve 0.32 gm. of the isomer melting at lo8^
100 cc. CiHtOH dissolve 0.42 gm. of the isomer melting at ia8^.
PICBIC ACID C«Hs.OH.(NOi)t 1.2.4.6.
Solubility in Water.
CDolinaki — B«r. 38, 1836, '05; Findky — J. Ch. Soc 8x, xaxg, 'oaO
••.
80
SdicyUte.
1.38
6.66
Sulfate.
very soluble
«
25
60
25
7.87
25
II. 6
«
25
0-57
0.
083
Gms.
C«H,J
^jpr per xoo
Grains
Gms. CaHiNj
Solution.
1O7 per xoo Gnuns
Solution.
Water.
Water.
0 0.67
(D.)
0.68 (D.)
1 .05 (F.)
60 2.77 (D.)
2.8l(D.)
3I7CFJ
10 .80
0.81
1. 10
70 3 -35
3-47
389
20 1. 10
I. II
1.22
80 4.22
4.41
4.66
30 1.38
1.40
^5S
90 5-44
S-72
S-49
40 1.75
1.78
1.98
100 6.7s
7.24
6.33
50 2.15
2.19
2-53
Dolinski does not refer to the previous determinations of Findlay.
100 gms. H2O dissolve 1.525 gms. C«Ht.OH.(N0^)t at 30^ and 1.868 gms. at 40^.
(Karplus, iSK>7*)
100 gms. HiO dissolve 1.45 gms. C«Hj.OH.(NOt)i at 20'. (Sisley, 1901.)
100 gms HiO containing 5 gms. HsSOi per liter, dissolve 0.61 gm. C6HiOH(NOi)t
at 20^ (Sisl^, igoa.)
100 gms. ethyl alcohol dissolve 8.37 gms. CeH»OH(NOt)i at 22®. (Timofeiew, 1894.)
100 gms. methyl alcohol dissolve 22.5 gms. C«HiOH(NOt)i at 22*. "
100 gms. propyl alcohol dissolve 3.81 gms. C5H»OH(NOi)i at 22®. "
100 gms. 95% formicacid dissolve 10.83 gms. C«HsOH(NOi)iat I9.8^ (Aschui, 1913)
493
PICBIC Acm
Solubility op Picric Acid in Water and in Aqueous Salt
Solutions at 25®.
(Levin — Z. phyaik. Ch. 55. 530, '06.)
One liter of aqueous solution contains 0.05328 gram mols. * 12.20
grams CeH,.OH(NO,), at 25^
G«mMd». Picric Add per Uter in Aq.SolttdcM of:
Gm. Mols. Salt
per Liter.
001
0.02
o.os
0.07
O.IO
0.50
1. 00
NaQ.
0.05524
o 05559
0.05729
0.05862
0.05902
0.0790
O.I180
NaNOs.
0.05529
0.05872
0.06632
0.07093
0.07670
NaiS04.
0.05604
0.05872
0.06632
0.07093
0.07670
liCl.
0.05480
0.05558
0.05703
0.05878
0.06132
Li9S04.
0.05661
0.06053
0.06691
0.07013
0.07437
0123
0.149
NH«a.
0.05487
0.05540
0.05771
0.05865
Gm. Moll.
Sak per Liter.
O.OI
0.02
0.05
0.07
O.IO
050
1. 00
'Grams Picric Add per Liter in Aq. Solutions of:
NaQ.
12.66
12.74
13.12
13-43
13 52
18.09
26.98
NaNOt.
M.67
13 -45
IS 19
16.25
17 -57
NaaSO«.
12.83
13
15
16
17
Gm. Mols. Picric Ac. per Uter Solution.
St ■
per
Sugar
' Uter.
Gm. Mob.
O.IO
0.25
050
1. 00
o. 05 202
0.04978
0.0482
0.0443
Gms.
11.92
11.40
11.04
10.15
45
19
25
57
ua.
"55
12.74
13.06
13 -47
14.05
UsS04.
12.97
13-87
15-33
16.06
17.04
28.18
34 14
NH4CL
"•57
.69
12
13
13
22
44
Solubility in Aq. Cane Sugar.
Solubility in Aq. Grape Sugar.
Sp. Gr.
Solution.
I. 0122
I .0319
1.0654
1. 1294
Gra. Mols.
Grape Sugar
per Liter.
O.IO
0.25
0.50
1. 00
Picric Acid per liter Sol.
G. Mols.
00530
0.0521
0.0509
0.0474
Gms.
12.14
"•93
11.66
10.86
Solubility op Picric Acid in Absolute Alcohol.
(Behrend — Z. physik. Ch. io» 265, V.)
100 gms. sat. solution contain 5.53 grams CeHjNjOy at 12.3®, and
$•92 grams at 14.6^. Sp. Gr. of the latter solution * 0.8255.
Solubility of Picric Acid in Benzene.
(FlndlayO
Mols.
CaHsNjOr
per 100
Mols.CaHs.
1.26
1.83
2.48
3-25
4 30
4.60
7.26
t:
Gms.
QHsNsO,
per 100
Gms-CA
5
3 70
10
S-37
IS
90
as
7.29
9-56
12.66
96.5
SS
13 51
dx.38
Gms.
Mols.
t*.
QHtNgOj
CeHaNgOx
per 100
Gms.CeHs.
per xoo
MoU-CaH^
38 -4
26.15
8.88
45
33-57
11.40
SS
50.65
17.21
58-7
58-42
19.83
65
71-31
24.20
75
96.77
32-92
PICBIC Acm
494
SoLUBiLiTT OP Picric Acid in Aqueous Solutions of Hydrochloric
Acid at 25**.
(Stepuiow, 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.Ha
per Liter.
0.25
0.50
0.7s
I
1.47
2.20
2.94
CA.OH.(NO0t per Liter.
. *
Mols.
O.OI16
0.0079
0.0062
0.0054
0.0050
0.0051
0.0057
Gms.
2.66
1.80
1.42
1.24
1. 14
IIS
131
Mds. Ha
per Liter.
3.67
4.40
SI4
S-5I
S.87
6.24
6.61
CA.0H.(N0s)t per Liter.
Mob.
0.0068
0.0082
0.0098
0.0105
O.OII5
0.0123
0.0125
Gms.
i-SS
1.87
2.26
2.41
2.65
2.82
2.86
Solubility of Picric Acid in Ethbr.
(Bougaolt, 1903.)
Sdvent. t*.
Ether of Sp. Gr. 0.721 13
Ether of Sp. Gr. 0.725 (0.8 pt.HjO per 100) 13
Ether of Sp. Gr. 0.726 (i pt. H^O per 100) 13
Ether saturated with HjO 15
HsO saturated with Ether 15
Gms. C»H«N A per Liter*
10.8 (B.)
36.8
«
40
51-2
13 -8
((
100 parts of ether dissolve about 2.27 gms. picric acid at 15**. (S. 1905.)
^ chloroform " " 2
petroleum ether " " G.04 "
100 gms. sat. solution in pure ether contain 5 gms. picric acid at 20**. (Sisleyp 190a J
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 amyl alcohol contain i .755 gms. picric acid at 20^. **
Distribution op Picric
Water and Amyl Alcohol.
(Hen and Fischer — Ber. 37> 4747t W)
Acid at 25** bbtwben:
Water and Toluene.
(H. and F.~ Ber. 38, xx4a, '05.)
MOlimob CeHaNsOr
Gms. CsHtNsOr
Millimols CeHaN»Or
Gms. CsHsNsOr
per
xocc.
per 100 cc.
per
10 cc.
per 1
00 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
0211 0.424
0.109
0.230
0250
0.527
01613
0.4127
0.369 0.946
0.163
0482
0.374
1. 104
0.1869
0.5182
0.428 I. 188
0.244
1.026
0.559
2 351
O.3161
1.079
0.724 2.473
0.389
2.347
0.891
5-380
0.4471
1.638
I 024 3.753
0.496
3-747
I 137
8.586
0.5624
2.189
1.288 5. 017
0.583
5135
I 336
11.770
0.6423
2.549
1.472 5-^39
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 PICBIC ACm
Distribution op Picric Acid at 25® bbtwbbn:
Water and Bromoform.
(Hen and Lewy — Z. Electrocfaem. iz» Sao. '05O
Water and Chloxof orm.
(H. and L.)
MOHmols C«HsNr«Or
per xo cc.
Gms. CeBsNsOr
per 100 cc.
MDlimob CeHtNiO,
per zo cc.
Gnu. r«H«N^
per xoo cc.
Aq. Bromoform
Layer. lAjer.
Aq. Bromoform
I^yer. Layer.
Aq. Chlorafarm
I^yer. Layer.
Aq. Chlaroform
Layer. Layer.
0.321 0.365
0.736 0.836
0 . 207 0 . 254
0.474 0.582
0.401 0.515
0.47s 0655
0.919 I. 180
1.088 I. 501
0.329 0.547
0.488 1.09
0.754 1.253
1. 118 2.498
0575 0-871
0.674 I. 14
1-317 I -995
1.545 2.612
0.561 I. 41
0.588 1.53
1.285 3.230
1.348 3.505
Distribution of Picric Acid bbtwbbn:
Water and Benzene. (Kuriloff, 1898.)
Water and Ether at 20*
. (Sialey, 190a.)
Mols. Picric Add per Liter:
Cms. Picric Acid per Liter:
Dist. Coef.
2.63
Aq. Layer.
0.0261
CA Layer.
0.0940
Aq. Layer. Ether Layer.
6.78 17.85
0.0208
0.0188
0.0779
0.0618
3.74 6.70
2.85 3.72
1.79
1.34
0.0132
0.0359
0.85 O.II
0.13
0.0097
0.0198
O.IO O.OOI
O.OI
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).
Frebzing-foint Data (Solubilities, see footnote, p. i) Are Given for
THE Following Mixtures:
Picric Acid + Dimethylpyrone. (Kendall, 1914.)
+ Resorcinol. (Philip and Smith, 1905.)
+ Thymol. (Kendall, 1916.)
-|- a Trinitrotoluene. (Giua, 1916.)
14
II
MethylPICRIC ACID aH(CH,)(OH)(NO,),, 1.3.2.4.6.
Solubelitt in Aqueous Solutions at 25^. (Kendall. z9xx.)
Aq. Solvent.
Water
" +Ligroin
" +Toluene
0.00895 nHCl
0.01593 nHCl
0.01013 n Picric Add
Normality of
Dissolved
Methvl Picric
Add.
Aq. Solvent.
0.01975 n 0 Nitrobenzoic Add
Normality of
Dissolved
Methyl Picric
Acid.
0.0080
0.01063
0.01072 .
0.02613*
O.OIOO
0.01019 0.00981 n Salicylic Acid
0.01059 0.01393 n " "
0.00641 HsO+£xcess of Salicylic Add
0.00487
0.00702
— nonnality of salicylic add + methylpicric acid.
PICROTOXm C»HmOi,.
1 00 gms. H»0 dissolve 0.4 1 + gm. picrotoxin at 20-25
. " pyridine dissolve 102 gms. " "
aq. 50% pyridine " 81
PUBLIC ACID (CHOsCCOOH),.
Distribution between Water and Ether at 25*^. (Chandler, 1908.)
(Dehn, 191 7-)
ti
(I
Mols. (CH,)b(C(X)H), per Liter.
Aq. Layer, a.
0.00998
0.00702
0.00480
0.00284
0.00179
Ether Layer, b.
0.01407
0.00979
0.00667
0.00380
0.00253
Dist. Coef. i
0.709s
0.7170
0.719s
0.7480
0.707s
Dist. Coef.
Corrected
for I<mi2ation.
0.670
0.670
0.663
0.663
0.653
PILOCABPINI
496
(Zaiai, 19x0.)
PILOCABPINI CiiHuNsO,.
100 cc. oil of aesame dissolve 0.3142 gm. CuHisNsOi at 20®.
PILOCARPINE HTDBOCHLOBIDE CnHi«N,0,.HCl, Pilocarpine Nitrate
CiiH,6NiOi.HNO,, and Piperine C17H19NO, in Several Solvents.
(u. s. P.. vm.)
Solvent.
Water
Alcohol
Alcohol
Chlorofonn
Ether
f.
25
2S
60
25
25
Gms. per xoo Gms. Solvent.
CuHHNAHa. CuH,«NA.HNO|. 'CdHi,NOi.
333
4. 35
9.09
0.18
25
1.66
6.2
insoluble
6.66
22.7
58.8
2.8
PINACOUN CH,.CO.C(CH,),.
Solubility in Water and in Aq. Acetone at 15**. (Peiinge, 1908.)
Per cent Acetone cc. Pinaoolin Dissolved
in Solvent. per 100 cc. Solvent.
o (= pure HjO) 2 .44
20 3.47
33 6.06
so 9.09
60 14.27
PINENE HTDBOCHLOBIDE CioHie.HCl.
100 gms. 95% formic acid dissolve 1.2 gms. CioHi«.HClat 16.8^. (Aacfaan. 19x3.)
PIPECOUNE C»H»(CH,)NH i and /.
F.-pt. data for mixtures of d and / pipecoline are given by Ladenburg and
Sobecki (19 10).
PIPEBIDINE CH,<(CHs.CH,),>NH.
Distribution between Water and Benzene at Ord. Temp. (Geoipevics, xgxs.)
Gms. Piperidine per:
Gms. Piperidine per:
as cc. H«0 lAytr. 75 cc. C(H« Lajrer.
35 cc. H|0 Lasrer. 75 oc. C»H« Layer.
0.891 2.339
1-299 3.589
I. 712 4789
0.1573 0.4127
0.256 • 0.674
0.409 1.088
0.674 I 746
PIPEBIDINE HTDBOCHLOBIDE CHs<(CHs.CH2)s>NH.HCl.
Solubility in Several Solvents. (Fmmdiich and Richards, 191a.)
Mols. Piperidine
Ha per Liter.
4.87
519
013
Sdvent.
Water
iC
Tetrachlor Ethane (sat. with H|0)
Nitrobenzene
Benzene
f.
o
25
o
25
25
25
0.29
0.00543
0.00102
MethylPIPEBIDINES 2-, 3., 4., n Methyl, etc.
Data for the reciprocal solubility of 2-methylpiperidiae and water, 3-methyl-
piperidine and water, 4-methylpiperidine and water, nitrosopiperidine and water
and for »-methyipiperidine and water, determined by the synthetic (sealed tube)
method of Alexeieff, are given by Flaschner and MacEwan (1908) and by Flasch-
ner (1909) and (1908). Similar data for n-ethylpiperidine and water and for n-
propylpiperidine and water are given by Flaschner (1908}.
497
PIPEBIDINE8
oa'Diphenyl PIPERIDINB8 CnHitN.
SOLUBILITIBS OF THE ACID SALTS OF oea' DiPHENYL PiPERIDINB AND OF ISO aai
DiPHENYL PiPERIDINE IN WaTER AT 25"*.
(Scholtz, 190X.)
PifMiriHifiA R**«
Gms.per xoo
Cms. Sat. Solution:
A,
nycaifUllIC l#i
*
kasait.
HBrSalt.
HI Salt.
HtSOiSalt.
a, <J Diphenyl Piperidine, m. pt. ;
'I** 0.8s
0.90
O.X2
6.31
laoafi/ Diphenyl Piperidine, liquid
3 02
I
0.72 easily soluble
PIPXBINE CnHi^NCV
(See also under Pilocarpine, preceding page
.)
Solubility in
Several Solvents.
Solyait
f.
Gms. CnHwNOiper
100 Gms. Solvent.
Authority.
Water
20-25
0
.01 (Dehn, 19x7.)
Ethyl Alcohol
95
2
. 0 (Timofeiew; 1894.)
Methyl "
95
4-4
II
Propyl "
95
2
•94
fi
Trichlor Ethylene
IS
9
. 83 (Wester and Bruins, 1914.)
Pjrridine
20-25
22
.46 (Dehn, 1917.)
Aq. 50% Pyridine
20-25
•
II
•39
li
PLATINUM ALLOTS
Solubility op Platinum Alloys in Nitric Acid.
(Winkler— Z. anal. Ch. 13, 369, '74-)
Appraz. Grams AD07 Diflsolved per 100 Grams HNOs Solution el
Pt in Allof. ;
i^98Sp.Gr.
z.a98Sp.Gr.
LiQoSp.Gr.
- ^
x.a98Sp.Gr4
Pt and Silver
10
S7
44
69
37
u
5
69
57
SI
35
ti
2 5
62
61
69
• •
u
I
75
70
76
• •
Pt and Copper
10
46
27
II
SI
u
s
36
34
14
41
tt
2-5
51
40
30
u
I
52
41
37
Pt and Lead
10
7
9
8
, ,•
<i
S
8
9
10
((
2-5
22
17
IZ
u
1+
21
18
^3
Pt and Bismuth
10
14
19
4
3
li
5
21
20
6
18
li
2-5
25
42
8
. •
u
I
49
64
10
• •
Pt and Zinc
zo
10
II
19
5
u
5
16
12
6
II
u
2-5
16
24
19
• •
u
z
20
32
37
• •
PLATIVUM BROMIDE PtBr«.
zoo grams sat. aqueous solution contain 0.41 gram PtBr4 at 20^.
(Halberstadt — Ber. I7» 9963, '84O
PLATINIO POTASSIUM BROMIDE K,PtBr,.
zoo grams sat. aqueous solution contain a. 02 grams KaPtBro at 20^.
(Halberstadt^
PLATINUM CHL0BIDE8
498
PLATINIC DOUBLB CHLORIDES of Ammonium, Caesium, Potassium,
Rubidium and Thallium. (Data for each separately.)
Solubility in Water.
(CroGkes — Chem. News 9» 37i 205, '64; Bunaen — Pogg. Ann- zz3b 337t '6zO
O
10
ao
30
40
SO
60
70
80
90
zoo
Grams per 100 Grams Water.
(NH«)aPtCl«.
666 (is^)
as
CssPtOe.
0.024
0.050
0.079
0095
O.IIO
0.143
0.177
0.213
0.251
0.291
0332
0377
KsPtOa.
0.74
090
1. 12
1.26
1. 41
1.76
2.17
2.64
319
3-79
4-45
S-iS
RbsPtC3e.
0.184
0.154
O.14I
0.143
O.I4S
0.166
0203
0-253
0.329
0.417
0.521
0.634
TlsPtdt.
• • •
0.0064 (15*0
0.050
Solubility of Potassium Chloroplatinatb in Water and in Aqueous
Solutions of Potassium Chloride and of Sodium Chloride.
(Archibald, Wilcox and Buckley, 1908.)
Solubility
in Water.
In Aq.
f.
Gms. KiPtCU
per xoo Gms.
H,0.
Gm. Mols.
KG
per Liter.
0
0.4784
0.20
10
0.5992
0.25
20
0.7742
0.50
30
I
I
40
1-355
2
60
2.444
3
80
3-7"
4
100
5-030
sat.
KCl at 20*.
In Aq. NaCl at 16**.
Gms. K,PtCU
Gm. Mols. Gms. K,PtCIi
per xoo Gms.
NaCl per xoo Gms.
Solvent.
per Liter. Solvent.
0.0236
0 0.672
0.0207
0.05 0.700
0.0109
o.io 0.729
0.0046
0.25 0.758
0.0045
0.50 0.775
0.0043
0.75 0.791
0.0042
I 0.805
0.0034
2 0.834
Solubility of Potassium Chloroplatinatb in Aqueous Solutions of
Methyl Alcohol and of Ethyl Alcohol at 20®.
(Archibald. Wilcox and Bockky, 1908.)
Wt. Per cent
Alcohol in
Solvent.
O
S
10
20
30
40
Gms. KsPt(n« per xoo (xms.:
Aq. CH,OH.
0.7742
0.535
0.412
0.264
O.183I
O.I165
Aq. CH»OH.
0.7742
0.491
0.372
0.218
0.134
0.076
Wt. Per cent
Alcohol in
Solvent.
50
60
70
80
90
100
Gms. KaPtC^ per 100 Gms.:
Aq. CHiOH.
0.0625
0.0325
0.0182
0.0124
0.0038
0.0027
Aq. CHiOH.
0.0491
0.0265
0.0128
0.0085
0.0025
0.0009
100 gms. aq. 8.2% isobutyl alcohol dissolve 0.625 gm. KsPtCU at 20^.
100 gms. aq. sat. isobutyl alcohol dissolve 0.318 gm. KsPtCU at 20^.
(Archibald, Wilcox and Buckley, 1908.)
One liter of 55% alcohol dissolves O.I 50 gm. (NHOtPtCUat 15-20^ (Freseoius, 1846.)
76% ** " 0.067 "
95% " " 0.0037"
If
««
It
<4
II
44
499 PLATXNUIE CHL0BIDE8
Distribution of Platinum Chloride between Water and Ether at
Ord. Temp. (Myiius. 1911.)
When I gm. of platinum as chloride is dissolved in 100 cc. of aq. 10% HCl 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% HCl, approximately the same per cent of Pt enters
the ether layer.
100 cc. anh)rdrous hydrazine dissolve i gm. platinic chloride, with formation of
a black precipitate at room temp. (Welsh and BnxknoD, 19x5.)
ChloroPLATINATES of Hydrocarbon Sulfines.
Solubility op Each in Water at 16®. (StxOmhoim. 1900.)
CUoiDplatinate. Cms. Sak per
/ ^ \ 100 Gins.
Name. Formula. Sat.*Solation.
Trimethyl Sulfine Chloroplatinate
Dimethyl Ethyl Sulfine Chloroplatinate
Methyl Diethyl Sulfine Chloroplatinate
Triethyl Sulfine Chloroplatinate
(CH,)sS]2PtCla 0.47
(CH,),(C,H)S]J>tCl« 3.43
CH,(C2H6),Si,PtCl« 2.42
(Cai)8S],PtCl« 1.98
Similar results for more complex sulfines are also given.
PLATING AMINES.
Solubility in Water. (Cieve, 1866 ?)
Amine. Formula. Gms. per 100 Gms. HiO.
Platino Semi Diamine Chloride p^ ^ ajrH,),.Cl o . 26 at o", 3 . 4 at loo"
Chloro Platino Amine Chloride aa>t<5J^jg o. 14 at o^ 3 at ioo<>
Chloro Platino Semi Diamine Chloride CUPt(NHi)2Cl o . 33 at o**, i . 54 at 100**
FLATINOUS NITRITE AlAMONIUM COMPOUNDS.
Solubility in Water. (Tschugaev and Kiitinovie. 1916.)
When ammonia is added to a cold solution of potassium platinonitrite a copious
precipitate of the composition Pt2NHi(NOi)8, 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-
NH, NOi
scribed, corresponds to the cis form of dinitro diammonio platinum, v Pt C
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. H^O.
f.
eft5PtaNH|(N0ft)t.
IraiuPtaNHaCNO^f
[Pt4NH,lIPt(NO0«l.
25
0.083
0.063
O.OII
63
0.66
0.49
• • •
74-4
• « «
0.81
• m •
95.
2.32
1. 85
• ■ •
Determinations of the solubility of several mixtures of the ds and trans com-
pounds in water are also given.
PONCEAU (Free Acid) CioH7N:N.CioH4(OH)(SO,H),.9H,0.
Solubility in Several Solvents at 23.^ (Sisi^, xgoa.)
Solvent. Gms. Ponceau per Liter.
Water 209.6
" + s 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 I8^
POTASSIUM
500
POTASSIUM Ks.
Solubility of Potassium in Liquid Ammonia. (Ruff aad Gdaei, 19064
^ Mols. NHa to Db-
* * Mlve I Gm. Atom K.
— 100 4.82
-SO 4-79
o 4-74
SOLUBILITT OF POTASSIUM IN MeLTBD KOH. (von Hnreqr. i909-)
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.
Gnu. K per xoo Gm. KOH.
7.8-8.9
3 -4
2 -2.7
oS-i-3
f.
480
600
650
700
POTASAMMONIUM K,(NH.)i.
100 gms. liquid ammonia dissolve 99.5 gms. Ki(NHi)i at o* and 97 gtaa. at
+8.44'
POTASSIUM ACETATE CH,COOK.iiH,0.
Solubility in Water. (Abe, zgn.)
Goaimia, 1906.)
f.
O.I
S
10
IS
20
2S
30
35
38
40
Gms. CIItC(X)K
per zoo Gms. Solid Phaie.
f.
216.7
223.9
233 -9
243 I
269.4
283.8
301.8
314.2
323 -3
Gms. CH«(XX)K
wt zoo Gms.
H«0.
Solid Phaie.
aCH|C00K.3H«0 4I
41 .3 tr. pt.
u
M
U
If
ff
ff
(I
fl
If
42
4S
SO
60
70
80
90
96
327
■ •
329
332
337
350
364
380
396
406
a CH«C(X)K.3H/>
+2CH,C00K.H/)
3CH,COOK.HdO
fl
2
3
8
I
3
S
(I
If
M
«4
•I
ff
M
O
20
40
so
60
Vo C,H»OH
>olveot.
70
80
90
9S
100
dn of Gms. CH«CCX)K per
Sat. Sol. zoo Gms. SolveoL
Solubility of Potassium Acetate in Aq. Alcohol Solutions at 25*. (SeidcU,'ia)
Wt. % CH»OH
in Solvent.
219.6
219.6
192.4
171. 8
147. s
dn of Gms. CHaCOOK per Wt.
Sat. Sol. zoo Gms. Solvent. in
1. 417
I 363
1.302
1.260
I. 210
1. 156
1.08s
0.990
0.922
0.850
118. 3
87.6
S2.9
34.2
16.3
F.-pt. data for potassium acetate + acetic acid (Vasilev, 1909);. potassium
acetate + sodium acetate (Baskov, 191 5).
POTASSIUM SulfoANTIMONATE K,SbS4.5H,0.
S(H.UB£LITY in Water. (Donk, xgoS.)
Gms. K«SbS|
(Baskov, I9i5<)
f.
\JIZ1S. ISkjODk
ZOO Gms. Sa
- 1-3
95
- 2.6
17. 1
- 4
24.2
- 7.2
35-4
— 10.6
42.9
-13s
48.8
-18.S
52.6
-28.8
59-6
Gms.K,SbS|Mr golid Phase.
loe
-34
— 10
- 4.S
o
+ 10
30
SO
80
zoo Gms. Sat.
62
69.1
7S-4
76.2
7SI
77-7
79.2
1.
Solid Phase.
Ice+K«SbS«.6H^
K«SbS<.6Hs0
fl
K<SbS4.sH|0
M
«
K^bS«.3HdO
<«
501 POTASSIUM SulfoANTIMONATB
S(X.UBiLiTT OF Potassium Sulfoantimonate in Aq. Solutions of
Potassium Hydroxide at 30** and Vice Versa.
(Donk, 1908.)
Gms. per zoo Gms. Sat. Sol.
Cms. per zoo Gms. Sat. Sol.
KiSbS,.
KOH.
ooua raaae.
K«SbS«.
KOH.
■s oouu raaae.
75
0
E<SbS«.5H|0
19.8
40.5
KaSbSi
68.4
3-4
K,SbS4.3H^
"S
49-9
" +KOH.2H1O
S6.8
II
f(
9-4
49-9
KOH.aH|0
50-9
16. 1
E,SbS«
0
56.3
M
37-7.
'S-5
11
Solubility of Potassium Sulfoantdionatb in Aq. Ethyl Alcohol.
(Donk, Z908.)
Results at so"*.
Solid Phaie.
E<SbS«.5H^
it
Results at 10^.
Gms. per zoo Gms. Sat. Sol.
K«SbS«. C|H»0H.
o 94
o 90.5
Two Uquid Layers Formed Heze.
69.2 0.8
76.1 O
Composition of the Liquid Layers.
Gms. per zoo Gms.
Gms. per zoo Gms. Sat. Sol.
K«SbS<.
O
CAOH.
97
SoUd Phase.
K«SbS|.3H|0
u
Two Liquid Layers Fonned Here.
7SI o
ft
Composition of the Liquid Layers.
Gms. per zoo Gms.
Alcoholic Layer.
KiSbS4.
Aqueous Lajrer.
Alcoholic Layer.
O
2.2
4.2
27.4
CHsOH.
54. 7
46.9
16
KiSbS,.
67.4
49
45 -6
CiHiOH.
I.I
3-4
3.8
K«SbS4.
o
o
2.2
8.5
CaH«OH.
93.1
85.6
56.8
41. 1
Aqueous Layer.
£l«SbS4.
70.5
65.2
47.8
37.1
C,H«OH.
1.2
5.7
9.2
12.7 31. I
Solubility of Potassium Sulfoantimonate in Aq. Methyl Alcohol at 15^
(Donk, Z908.)
Composition of the Liquid Layers.
Cms. Sat. Sol.
SoUd Phase.
Gms. per zoc
1 Gms.
Gms. pec loo
Alcoholic Layer.
KiSbS«. CH^H.
Aqueoii
K,SbS«.
IS Layer.
' KiSbS,.
CHaOH.
ch^h.
OS
99-5
E^bS4
5 82. s
62. s
8
0.4S
99.5
(1
4.9 76.3
• • •
• • •
IS
93-9
If
7 66.9
• • •
• • a
1.8
92
<f
13-6 54
• • a
a • •
Two Liquid Layen Fonned Here.
19. I 45-5
a • a
a . •
62.7
7 . 5 K,SbS4.9H/>
. . • . • . _
311
31-3
68.4
3.5
tt
• . • * . •
41. 1
22.2
7SS
0
<f
• • . • a *
47.2
18.2
Two Liquid Layers Formed Heze.
• • • • • •
S7-3
II. I
o-S
98.1
<(
POTASSIUM (Dihydrogen) ARSENATE KHtAs04.
100 gms. sat. aq. solution contain 15.9 gms. KHtAsOi, or 100 gms. HsO dissolve
18.86 gms. at 6^. Sp. Gr. of solution » 1.1134. (Field, Z859.)
100 cc. sat. aq. solution contain 28.24 gms. KHsAsOi at about 7^
(Muthmami and Kuntze, Z894.)
100 gms. glycerol {di§ » 1.256) dissolve 50.1 gms. potassium arsenate at 15-16^
(Oasendowski, Z907.)
POTASSIUM BENZOATI
502
POTASSIUM BENZOATI KCrHsOt-aHsO.
S(H.UBILITY IN WATBR.
(PajetU. 1906. 1907.)
Gms. KCrHtQi per 100 Gms. Solution 41 . i
25-
42.4
33-3
44
SO-
46.6
POTASSIUM BORATES.
Solubility op Potassium Borates in Water at 30*.
(Dukelski — Z. anorg. Chem. 50^ 42. '06, oomplete refemioet given.)
Gnu. Sohitioo.
Bid.
Cms. per 100
Gms. Retidae
Solid
' KiO.
K«0.
BiOi.
Phase.
47 SO
• * •
• • •
• • •
KOH.SH1O
46
36
0
9»
46
13
9
03
K^3«0».aiH^
40
S»
I
25
41
63
9
71
••
36
83
I
80
39
90
13
19
M
32
74
3
SI
37
.33
14.
58
M
39
63
6
98
35
05
17
93
M
a4
84
17
63
30
03
21.
70
W
93
30
18
.19
36
84
31
49
K^3BfOft4HK>
16
31
13
10
as
.13
33
18
tt
II.
.78
9
.83
30
•57
26
43
H
9
18
8
00
33
38
31
30
•1
6.
33
9
13
30
87
31
06
M
7'
73
13
37
33.
31
36
24
K^.aBsO|4HsO +KsO.5Bs0|.8HiO
7'
81
13
38
17
50
34
18
t
7
71
13
31
II.
49
34
81
K^.5BfOft.8H«0
7
63
13
38
13.
SI
40
•Sa
M
3
4a
7
S9
10
•77
37
35
M
I
80
4
IS
5
88
20
00
•«
0
SI
3
19
10
81
40.
89
tt
0
33
4
58
7
.72
34
31
Ki0.sBjO»^HK) + B(OH)i
0
3'
4
46
3
91
30-
68
*«
• <
> •
3
54
• <
1 •
• <
1 •
••
POTASSIUM MetaBORATE KBO,.
Fusion-point data for potassium metaborate + sodium metaborate and for
potassium metaborate + potassium metaphosphate are given by van Klooster
(1910-11).
POTASSIUM PerBORATBS, 2KB0s.H,0, 2KB0s.Hs0t.
Solubility of EIach in Water.
(v. Girsewald and Wolokitin, 1909.)
Boimte.
2e:bQs.HjiO
«
2e:bQs.ha
% Active O in
Borate.
14.93
14 -93
20.84
V.
o
IS
15
Gms. Salt
Gms
alt per xoo
.Water.
I-2S
2.50
0.70
POTASSIUM (Fluo) BOBIDE KBF4.
100 gms. HfO dissolve 0.44 gm. KBF4 at 20^, and 6.27 gms. at 100^.
(Stdba, Z889O
503
POTASSIUM BBOMATI
POTASSIUM BBOMATI KBrOk.
Solubility in Water.
(Kxemers— 'Pogg. Aim.97> 5. '56; Rammelsberg — /Mf . 5& 79* '43; Pohl ~ Sitzber. Akad. Wias
Wien. 6b S95» 'sx-)
kO
G«D8. KBtO» per zoo Cms.
f.
Cms. KBrOs
per zoo Gms.
fc .
'Wfltrr. Solution.
"Water.
Sdution.'
0
31 30
40
13.2
II. 7
10
4.8 4.6
50
I7S
14.9
20
6.9 6-5
60
22. 'T
18.5
25
8.0 7.4
80
34 0
25-4
30
9-5 ^-7
100
50.0
33-3
Sp. Gr. of solution saturated at 19.5^ - 1.05.
Solubility op Potassium Bromatb in Aqueous Solutions op
Sodium Nitrate and op Sodium Chloride.
(Geffcken — Z. phyaik. Chem. 49^ 296. '04.)
In Sodium Nitrate.
In Sodium Chloride.
Grams per Liter. Mob. KBrOi
Grams
per Liter.
Mnb. KBrOi
NaNOj. KBrO,. Per Liter.
NaQ.
KBrOs.
per Liter.
0.0 78.79 0.4715
00
78.79
0.4715
42.54 96.01 0.5745
29 25
82.24
05220
85.09 108.6 0.6497
58 SO
93-87
0.5616
170.18 128.3 07680
117. 0
100.9
06042
255-27 150 -9 0.9026
I7S-5
104.3
0.6244
340.36 172.3 I. 031
234.0
106.9
0.6400
S(h.ubility op Potassium BROiiATs in Aqueous Solutions op Various
Compounds at 25°.
(Rothmund, 1910.)
Solvent, o.« Nonnal
Aq. Sol. of:
Mols.
KBrOiper
Gms.
KBrQiper
Uter.
Solvent, 0.5 Nonnal
Aq. Sol. of:
Mols.
KBrQiper
Liter.
Gms.
KBiQiper
liter.
Water alone
0.478
79.84
Dimethylpyrone
0.478
79.84
Methyl Alcohol
0.444
74.16
Ammonia
0.44s
74.33
Ethyl Alcohol
0.421
70.33
Dimethvlamine
0.384
64.13
Propyl Alcohol
0.409
68.31
Pyridine
O.41S
69.31
Tertiary Amyl Alcohol 0.383
63.97
Piperidine
0.396
66.15
Acetone
0.425
70.99
Urethan
0.433
72.33
Ethyl Ether
0.39s
65.98
Formamide
0.473
79.02
Formaldehyde
0.397
66.31
Acetamide
0.44s
74.33
Glycol
0.448
74.84
Glycocol
0.501
83.68
Glycerol
0.4SI
75.34
Acetic Add
0.456
76.17
Mannitol
0.451
75.34
Phenol
0.426
71.15
Grape Sugar
0.431
71.99
Methylal
0.405
67.66
Urea
0.477
79.68
Methyl Acetate
0.420
70.15
POTASSIUM BBOHIDI
504
POTASSIUM BBOMIDI KBr.
Solubility in Water.
(Awage cure from results of MfiiiaBcr — Z. anorg. Chem. 4^ 70, '05
'84; Ann. diim. tdiys. [tJ a* 526, '94; de Coppet — ibtd. [cj
SbaMcae — Phil. Tnns. 17& as. ^i
; Etud — Compc. rend. 98^ 143%
30^^x6, '83; Tuden and
Grams KBr pet 100 Grams
- 6-5
-8-5
— 10.5
-"-S
— 10
— 5
o
S
10
IS
30
25
Solution.
20.0
26.5
29 5
31.2
318
33-3
34-9
36.1
37-3
38s
39 S
40.4
Water.
25.0
35-7
41.8
45-3
46.7
50. o
S3S
565
S9S
62.5
65.2
67.7
30
40
SO
60
70
80
90
100
no
140
181
Grams KBr per 100 Grams
' Solvtian.
Water.
41.4
70.6
43 0
75 S
44. s
80.3
46.1
855
47-4
90.0
48.7
95 0
49.8
99.2
51.0
104.0
52-3
109.5
547
120.9
59-3
145.6
Solubility op Mixtures op Potassium Bromide and Ammonium
Bromide in Water at 25°.
(Fock — Z. Kryst. Min. a8» 357, '97.)
Grams per LJ
ter SobtioD.
KBr. '
Mol. per cent in Solution.
NHiBr. KBr.
Sp. Gr. of
Sdutioas.
Md. per cent in Solid Phaa
NH«Br.
NH«Br.
KBr.
0.00
558.1
0.0
100
1-3756
0.00
100
6.4
554.2
1.38
98.62
I -3745
0.26
99-74
24.64
536.5
5 29
94
•71
1-3733
1.27
98.73
51 -34
516.8
10.77
89
23
1. 3721
3.02
96.98
152.9
441.2
29.63
70
•37
1.37"
8.42
91.58
262.2
347-3
47.84
52
.16
1-3715
17.20
82.80
347.6
262.3
61.69
38
31
1-3753
27.98
72.02
381.4
260.3
64.03
35-
97
1-3753
32-53
67.47
417.8
232.2
68.61
31-
39
1.3766
39-45
60.55
4325
222.3
70.27
29.
73
1-3777
variable
variable
480.8
179.9
76.47
23
53
1.3766
98 -.53
1.47
577-3
0.0
100 .0
0.
.0
1.3763
100 .0
0.00
Solubility op Potassium Bromide at 25* in:
Aq. Solutions of KCl and Vice Versa. Aq. Solutions of KI and Vice Versa.
(Amadori and Pampanini, 19x1.)
Gms. per 100 Gms. H^.
(Amadori and Pampanini, 19x1.)
Gms. per xoo Gms. H|0.
KBr.
68.47
62.26
58.50
52.45
45.42
38.70
26.62
12.94
O
(See also next page.)
KCL
o
5-. 43
8.46
12.48
17.17
21.23
25.88
31.02
36.12
KBr.
53.21
42.32
34.14
30.08
29.62
22.15
21.88
18.54
o
Kir
35.92
66.63
95.36
119.52
119
127.10
127.31
130.61
149.26
505
POTASSIUM BBOHIDI
Solubility of Potassium Bromide in Aqueous Solutions of
Potassium Hydroxide.
(Ditto — Compt. rend, za^t so* '97.)
Gnins per
1000 Grams HjO.
Grams per 1000 Grams HsO
KOH.
36 -4
177.2
231 I
KBr.
558.4
433-6
358.1
281.2
KOH. KBr.
277.6 248.1
434.7 137 I
579.6 64.8
806.9 33.4
Solubility op Mixtures op Potassium Bromide and Chloride and
of Mixtures op Potassium Bromide and Iodide in Water.
(Etard — Ann. cfaim. phys. [7] 3, 375, '97.)
Mixtures of KBr and KCl. Mixtures of KBr and KI.
«•
Grams per 100
Gms. Solution.
Grams per 100
Grams Solution
• •
KBr.
KO.
^ KBr.
KI.
—20
17s
10. s
9.2
42.5
0
21-5
10.8
9.9
45-3
10
23.2
II. 0
10.2
46.6
20
24.8
II. 2
10.5
47-5
25
255
"•3
10.7
48.0
30
26.3
II .4
10.9
48.6
40
28.0
"5
II. 2
49.6
60
30.6
II .8
II. 9
51 -3
80
33-4
12. 1
12.6
52.7
100
35-7
12.6
13-2
53-8
120
38.0
12.9
14.0
54.8
ISO
40.6
13-4
14.9
55-5
Solubility op Potassium Bromide in Aqueous Solutions op
PoTASsrutf Chloride, and op Potassium Chloride in Aqueous
Solutions op Potassium Bromide, at 25.2^.
(Touxen — Compt. rend. 130^ zasa, '00.)
KBr in Aq.
KCl Solutions.
KCl
in Aq.
KBr Solutions.
Mols. per liter.
Grams
per Liter.
Mob. per Liter.
per liter.
KQ.
KRr.
KG.
KBr.
KBr.
KQ.
KBr.
KQ.
0.0
4.761
0.0
567.0
0.0
4.18
0.00
3" -8
0.67
4.22
500
502.5
0.49
3 85
58.4
287.2
0.81
4. IS
60.4
494.2
0.85
3 58
101.3
267.1
I -35
3 70
100.7
440.7
I -31
3-19
156.1
238.0
Z.48
3-54
no. 4
421.6
1.78
2.91
211. 9
217. 1
1. 61
3-42
Z20.0
407.2
2.25
2.58
268.0
192.4
1.70
3-34
126.8
397-7
2.69
2.33
320.4
173 -8
2.46
2.50
183.5
297-7
3-775
0-525
281.6
625-3
POTASSIUM BROHIDI
506
Solubility op Potassium Bromide in Aqubous 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^ go8» '00.)
KBr in Aqueous KNOa Solutions. KNO, in Aq. KBr Solutions.
Mob. per Uter. Gmns jper Liter. Mols. per Liter. Grams per
tSCh. KBr.
tNQi.
KBr.
KBr.
KNO^.
KBr.
KNOfe.
Results at 14.3*.
Results at 14.10*.
00 4-33^
0.0
515-9
0.0
2.228
0.0
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
0.784
I 835
93-4
185.7
I -235 3-939
124 9
469.1
1.092
1.730
130.0
175 0
1-577
1-587
187.8
160.6
Rcsttlts at a5.a*.
2-542
1.406
302.7
142.2
0.0 4.761
0.0
566.2
3-536
1.308
421. 1
132-3
O.I3I 4.72
13 -3
561.0
Results at 95.2*.
0.527 4.61
53-3
549-1
0.0
3-217
0.0
325-5
0.721 4.54
72.9
540.8
0.38
3.026
45-3
306.2
109 4 -475
no. 3
533-0
0-93
2.689
no. 8
272.0
1. 170 4.44
118. 4
528.8
1-37
2.492
163. 1
252.2
1-504 4-375
152.2
521. 1
1.208
2.216
143-8
224.3
2.87
1.958
341.8
198. 1
3-55
1.807
422.8
182.8
Solubility of Potassium Bromide
IN Alcohols at
25^
(de Bmyn — Z. physik. Chezn
I. xo» 783. *
93; Rohland —
- Z. anorg. Chem. i8| 337
.•98.)
Alcohfll.
Grams KBr Dissolved by zoo Gms.
. . -A_ .
Alcohol at:
Room Temp. (R.).
»i
f (de B.).
Methyl Alcohol
I .
92
I 51
Abs. Alcohol
Ethyl Alcohol
0.
28 (Sp.
Gr. 0.81)
0.13
tt
Propyl Alcohol
0.
055
• • •
Solubility op Potassium Bromide in Aqueous Alcohol.
(Taylor— J. Physic. Ch. z« 7*4. '96-*97.)
Wt. per cent Alcohol
in Solution.
O
5
10
20
30
40
50
60
70
80
90
Results at 30^.
Gms. KBr
££L
TOO Gms.
Sat. Solution.
41.62
38.98
36.33
31.09
25.98
21.24
16.27
n.50
6.90
3 09
0.87
Solvent.
71
67
63
56
50
44
38
32
24
15
8
30
25
40
40
15
95
85
50
70
95
80
Results at 40^.
Gms. KBr per 100 Gms.
Solvent.
Sat. Solution.
43-40
85
40
38
33
28
23
18
xoo gm. acetone dissolve 0.023 gm.
13.02
7.98
3-65
1.03
KBr at 25^
37
27
32
22
II
76.65
72.70
69.00
62.30
56.45
50.46
4425
37 40
28.90
18.95
10.45
(Krug and McElioy — J. anal. Chem. 6b 184, '90^
507
POTASSIUM BBOHIDI
SOLUBILITT OF POTASSIUM BrOMIDE IN DiLUTB AQUEOUS ETHYL AlCOHCH^.
Results at 0"*.
(Armatroiig and Eyre, igio-xz.)
Wt. % CsHdOH
in Solvtent.
O
1. 14
2.2$
4.41
8.44
Cms. KBr per
100 Gms. Sat. Sol.
34.92
34-35
32.96
3199
2943
Results at 25"".
(Annatroog, Eyre, Hussey and Paddison, 1907.)
Wt % CHiOH
insolvent.
O
1. 14
2.25
4.41
12.14
18.73
Gms. KBr per
zoo Gnu. Sat. SoL
40.78
39.98
39-54
38.41
34.97
30.91
dm. of Sat. SoL
I . 3824
1.3727
1.3634
1.3443
I.281S
1.2322
100 gms. methyl alcohol dissolve 2:17 gms. KBr at 25^ (Turner and Btssett, 19x3.)
•^ ethyl " " 0.142 gm.
propyl " " 0.035
amy! " " 0.003
II
II
II
II
II
Sqlubilitt of Potassium Bromide in Aqueous Sch^utions of Methyl
Alcohol at 25®.
(Hen and Anders, 1907.)
Wt.% CH^H Gnu. KBr per
in Solvent. 100 cc. Sat. Sol.
o 56.04
10.6 46.28
30.8 29.98
47.1 19.28
iy of Sat. Sol.
1-3797
1.300
1. 159
1.058
Wt. % CHiOH Gms. KBr per
in Solvent. 100 oc. Sat. SoL
64 10.35
78.1 5.24
98.9 2.74
100 1.69
dju of Sat. SoL
0.9801
0.8906
O.8411
0.8047
The solubility of potassium bromide in methyl alcohol at the critical tem-
perature b given by C^entnerszner (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, 19x3.)
100 cc. anhydrous hydrazine dissolve 60 gms. KBr at room temp.
(Welsh ana Broderson, 19x5.)
100 gms. hydrozylamine dissolve about 44.7 gms. KBr at I7^-I8^
(de.Bruyn, X899O
Solubility of Potassium Bromide at 25'
(Herz and Knoch, 1905.)
IN:
cc. Acetone
per xoocc.
Solvent.
O
20
30
40
50
60
70
80
90
100 CC.
0.139 gni.
Aqueous Acetone.
Per 100 cc. Sat. Solution,
tiillimob
KBr.
481.3
366.7
310.5
259
202.9
144.9
95.3
46.5
10. 1
Gms.
KBr.
57.3
43.67
36.98
30.85
24.16
17.22
"35
5.54
1.20
Gms.
H^.
80.6
695
62.97
55-60
47.60
39.15
29.78
20.10
10.15
Sp. Gr.
tions.
sp.
Sohxl
1.3793
I . 2688
I.2118
I. 1558
I. 0918
1.0275
0.9591
0.8942
0.8340
Wt.%
^ Glycerol
in Solvent.
O
13-28
25.98
45.36
54.23
83.84
100
Aqueous Glycerol.
KBr per xoo cc. Sol.
« * . »
Millimols. Gms.
481.3
444.3
404
340.5
310.4
219.25
172.65
57.32
52.91
48.11
40.55
36.98
26.11
20.56
Sp. Gr.
Solutions.
1.3793
1.3704
1.3655
1.3594
1.3580
1.3603
I. 3691
sat. solution of potassium bromide in furfurol (CiHaO.COH) contain
KBr at 25^ (Walden, X906.)
Fusion-point Data for Mixtures of KBr and Other Salts.
KBr + KF
KBr + KCl
KBr + KI
KBr + AgBr
KBr + NaCl
KBr + KOH
(Kumakow and Wrzesnewsky, x9xa; Ruff and Plato, 1903.)
(Wrzesnewsky, x9X2; Amadori and Pampanini, xgxx; Ruff and Plato X9Q3O
II
«
If
M
(Sandonnini, xgxa.)
(Ruff and Plato, x9os.)
(Scaipa, X9X5.)
POTASSIUM BUTTRATB
508
POTASSIUM BUTTRATI C,H7CCX)K.
100 gms. water dissolve 296.8 gms. CiHyCOOK, or 100 gms. sat. solution oon-
tain 74.8 gms. at 31.25^.
100 gms. of an aq. solution saturated with sugar and CiHtCOOK contain
49.19 gms. sugar -|- 34.78 gms. CiHtCOOK + 16.03 gnw. H|0 at 31.25*.
(KflUer. 2897.)
POTASSIUM CAMPHORATES.
Solubility in Aqusous Solutions op d Camphoric Acid at 13.5-16* and
Vice Versa.
Gms. per xoo
Gms. Sat. Sol.
Soiki Phaie.
Gms. per 100
Gms.Sat. SoL
Solid PlMK.
CtHiiCCOOH),.
C|#Hm04Ki.
biHMCCOOH),.
CiiHh04K«.
0
66.6s
C»HuO«K.
2.90
32.84
C»H,AK.Q|H,A
0.90
69.69
C»H,^4K
3-20
29 -39
II
«
X
69
(1
3 30
28.56
CiiHtf04K.3CttHiA
1. 10
66.79
*f
3-20
27.32
u
0.90
66.65
QiH,/>«K.H^
3.20
22.77
M
I 50
62.37
M
310
21.66
M
2.60
S9-34
M
2.90
12.97
«
3 -20
58-37
ft
2.90
"•73
•1
3.20
58.09
•I
310
"59
ilQHM(GOOB),
3.20
52.71 1
C»HiAK.C»H,A
2.90
9.66
M
3.20
48.43
*i
2.80
8.14
l<
2.80
47-88
u
2.50
6.76
«
2.80
42.36
II
2.30
6.07
U
3
35-60
w
2
4. 55
M
2.85
34-77
M
0.621
0
M
CwHiAKi » DipoUssium d camphorate. CMHM04K.CipHtfQ| ■ MonopotaaBiam d dicamphocate.
CaHu04K » Monopotassiumdcampborate. CMHuOiK.jCieBLMOi - Monopotsiwhim d tetracamphoiMte.
POTASSIUM CARBONATE KsCOt.2HsO.
Solubility in Water.
(de Coppet, 1873; Meyerhoffer, 1905; Osaka. 19x0-12. Kiemann and Zitek, 2909; de Waal, 1910;
Muldor, 1864.)
Gms. KiCOi
t*. per zoo Gms.
Sat. Solution.
Solid Phase.
r.
Gms. KiCOk
per 100 Gms.
Sat. Solution.
Solid Phase.
— 10 21.3
loe
40
53-9
K«C0|.3H^
-20 31
II
50
54.8
M
-30 36.9
M
60
55-9
H
—36.5 Eutec. 39.6
" +K|CQg«H,0
70
57.1
H
— 6.8 tr. pt. 50.9
E,COkJcH«0+K«COk.aH|0
80
58.3
a
0 51 -3
K|C0k.2H^
90
59-6
M
+10 52
II
100
60.9
m
20 52.5
II
no
62.5
m
25 52.8
II
120
64.4
u
30 53-2
•1
130
66.2
M
Single determinations, not in good agreement with the above, are given by
Kdhler (1897), by Engel (1888), and by Greenish and Smith (1901).
POTASSIUM BiCARBONATE KHCO,.
Solubility in HiO. (Dibbeu, 1874.)
t®. o 10 20 30 40 60
Gms.KHCQsperiooGms.Sat.Sol. 18.3 21.7 24.9 28.1 31.2 37.5
100 gms. sat. aqueous solution contain 18.7 ems. KHCOi at o® {d » 1.127)
(Engel, 1888); 23.7 gms KHCO* at 15** (Greenish & Smith, 1901); 26.3 gms. at
20** (de Forcrand, 1909).
509 POTASSIUM CARBONATE
SOLUBILITT OF POTASSIUM BiCA&BONATE IN AQUEOUS SOLUTIONS OF
Potassium Cakbonatb at o^ CBasd, i88S.)
Milligram Mob. per i cc. Solution. Sd. Gr. of Grains per loo cc. Soludoo-
*KaCX)^
KHCOi
Solutions.
KaCO».
KHCOi.
O.O
21.15
I 133
0.0
21.2
17.14
15-28
1. 182
II.8
IS -3
24.10
12.65
1.20
16.7
12.6
34.50
10.25
1. 241
23.8
10.3
49.20
7-55
1.298
34 0
7.6
62.14
5-86
I 350
43 0
5-9
74.60
4.90
1.398
51.6
4-9
87.50
3-75
1.448
60.5
3.8
"7-75
00
i-54«
81.4
0.0
Solubility of Potassium Carbonate in Aqueous Solutions of Potassium
Chloride and of Potassium Hydroxide at 30®. (de Waal, 19x0.)
Results for KsCO. + KCl. Results for KsCOs + KOH.
Gms. per loc
i Gna. Sat. Sol.
Solid Phase.
" +Ka
KQ
u
M
Gms. per 100
Gms. Sat. Sol.
Solid Phase.
KtC0k.ziH^
If
" +KOH.aHdO
; KOH.aHdO
53.27
52.22
51.66
1.64
0
KCL
0
1.03
1.07
26.22
28.01
'k,co,.
53.27
2.50
2.05
0
KOH.
0
53.77
55.14
55-75
100 gms. HfO dissolve 10.76 gms. KsCOi + 2.66 gms. KNOi at 10° when both
salts are present in excess. (Kxemann and Ziiek, 1909.)
100 gms. HsO dissolve 10.53 gms. KsCOi + 6.12 gms. NaiCOs 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 KiCOs + KNOi + NasCOt + NaNOi, 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 KtCOi + BaSO* ^ KsSOi + BaCO» at 25*,
80" and 100** are given by MeyerhofFer (1905).
An aqueous solution, simultaneously saturated with KsCO».2HfO, KiSOa and
BaCO», contains 53.1 gms. KsCOa + 0.023 S^- KsSOi at 25^. (Meyerhoffer, 1905.)
Equilibrium in the System Potassium Carbonate, Ethyl Alcohol and
Water at 23**-26". (FranWorter 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 KiCOi in spe-
cially prepared conjugated lic[uids. 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 zoo Gms. Sdution.
A.
Gms.
per zoo Gms. Solution.
A
K«C0|.
CHjOH.
njo.
KtCQ,.
C,H,.
H|0.
0.095
90.65
9.255t
53.6
0.28
46.12!
0.241
72.7
27.059
39."
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
19.15
13.2
67.65
10.35
27
62.65-
18.18
14.7
67.12
14.2
20.5
65-3
* Plait point.
14.2
t Quad. pobt.
20.5
65.3*
The authcH^ give a complete summary of previous investigations of this system
by de Bruyn (1899, 1900); Bell (1905); Cuno (1908-09).
POTASSIUM CARBONATB
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 Bnxyn, 1900.)
Cms. per zoo Cms. Upper Layer.
Cms. per 100 Cms. Lower laytx.
• .
K.CQ^
QHiOH.
Hid.
-18
0.03
90.3
9-7
0
0.04
91.9
8.1
+17
0.06
91.5
8.4
35
0.07
90.9
9
SO
0.09
91.8
8.1
75
0.12
^1.4
8.5
EfCQ^
ch^h.
Hrf).
51.2
0.2
48.6
51.3
0.2
48.5
52.1
0.2
47-7
53-4
0.2
46.4
55.3
0.2
44.5
57-9
0.2
41.9
Equilibrium in the System Potassium Carbonate, Methyl Alcohol,
Water at 23**-26**.
(Fnmkforter and Ftary, 19x3.)
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
TOO Gms. Homogeneous Liquid.
Cms. per
A
KfOV
CHiOH.
H^.
K«C0|.
CHiOH.
HiO.
6.32
75.8s
17.83*
21.61
33.43
44.96
6.91
63.13
29.97
23.15
31.26
45
60
8.07
59.26
32.67
28.2s
23.82
47-
94
10.17
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.
t Lower quad, point.
The following results for the solubility of KsCOs in concentrations of aq«
CHgOH above and below those yielding liquid layers are also given.
Gms. per zoo Gms. Sat. Sol.
Gms. per zoo Gms. Sat. Sol.
CHiOH.
1.03
2.22
6.1
KaCQi.
51.39
50.33
49.05 (Lowerquad.pt.)
Two Liqxiid Layers Formed Here.
75.85 6.32 (Upper quad pt).
CHiOH.
85
89.2
91
93.6
94.3
K,COk.
2.05
1.56
1.98
2.7a
5.7
(Aba. (n]/)H).
Data for the binodal curves for this system at 17* and at 35* are given by
de Bruyn (1900).
^ 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.
(jms per zoo Gms. Upper Layer.
Gms. per
zoo Gms. Lower Layer.
V.
K,CQ^
CH/)H.
HiO.
K«CO,.
CHaOH.
HsO.
-30
21.7
42.2
36.1
• • •
. . •
• • •
—20
13.8
52.1
34.1
• • •
...
• • •
—20
12.4
• • »
• • •
44.2
8.2
47.6
0
7.6
66.3
26.1
46.3
6.7
47
0
7.4
■ • •
...
46.6
6.6
46.8
+17
6.2
69.6
24.2
48.3
5.7
46
35
5
72.9
22.1
SI
4.3
44.7
5"
POTASSIUM CARBONATB
EQtnLIBRIUM IN THB SySTBM POTASSIUM CARBONATE, NORMAL PROPYL
Alcohol and Watbr at 22"-26^
(Fxankforter and Frary, 19x3.)
The authors give the data for the binodal curve and the quadruple points
but tie lines were not located.
Gins, per xoo Gms. Homogeneous liquid.
Cms. per zoo Gms. Homogeneous Liquid.
So?
83.25
82.96
82.56
81.54
79.71
72.87
63.19
59.29
53.09
47-49
35. 41
4.i53t
Equilibrium in the System Potassium Carbonate, Isoprofyl Alcohol
AND Water at 20*,
(Frankfoxter 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.
pea: 100 gms. of homogeneous liquid (KsCOa + water + alcohol.)
K.CO,.
CtH/)H.
^•0*
52.9
0.02
47.08*
46.98
0.12
52.91
39
0.20
60.80
34.58
0.20
65.15
30.43
0.45
69.12
26.51
0.78
72.71
22.81
1.32
75.87
19.08
2.31
78.62
16.35
3.24
80.41
13.47
4.41
82.12
10.99
6.24
82.77
8.55
8.31
83.14
-
* Lower quad, point.
K,CO^
CsHvOH.
7.45
9.30
5-97
11.07
4.73
12.71
3.86
14.60
3. II
17.17
2.42
24.71
1. 91
34.90
1. 71
39
1.33
45.57
0.948
51.56
0.387
64.20
0.017
95.83
t Upper quad.
point.
Gms. per zoo
Gms. Alcohol + Water.
Gms. per
zoo Gms. Alcohol + Water.
K.CO^
AlcohoL
Water.
K.CO^
Alcohol.
Water.
44.844
2. 911
97.089
15.021
19.445
80.555
36.137
4.783
95.217
13.244
23.919
76.081
28.879
7.349
92.651
6.065
45. 397
54603
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, Z9Z5.)
Gms. per zoo Gms. Alcohol + Water.
Gms. per z(x> Gms. Alcohol + Water.
KtCQa.
Alcohol.
Water.
K.CQ,.
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
9309
90.691
2.020
54.487
45 • 513
16.354
15 037
84.963
1. 015
62.610
37.390
".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, X914.)
The binodal curve was very carefully determined and, in addition, data for the
quadruple points (solid KiCOs) 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 zoo Gms.
Upper Layer.
H,0.
Gms.
per
zoo Gms. Lower Layer.
K«C0i. (CHOiCO.
K«CO».
(CH^iCO.
H|0.
0.0024 96.4
3-5+t
52.4
trace
47. 6t
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
65
¥
14.77
13
72.23
10.5 20
69
10.5
20
69.5
•Plait pa
int.
t Quad, points.
POTASSIUM CARBONATI
512
Equilibrium in the System Potassium Carbonate, Potassium Diprofvl
Malonate and Water at 25°.
(M 'David, 190^10.)
A series of mixtures of K9CO1 + KC11H11O4 + HsO 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 Gnu. Upper Layer.
Gma.per
100 Gnu. Lower Lawyer.
K,COk.
KCiiHifOt.
1^0.
K.CQ,.
KC„H,A.
HiO.
4-05
65.1
30.85
42.6
0.4
57
4 9
59.8
35 3
40.7
0.4
58.9
5.6
53-5
40.9
35
05
64.5
7.2
50.5
42.3
33. 5
0.9
65.6
8.7
39-2
52.1
28.9
0.7
70.4
II
34 6
54.4
26.8
0.8
72.4
145
23-S
62
24.8
3
72.2
17
18.6
64.4
23.1
6.0s
70.8s
18.6
IS
66.4
21.7
«.7
69.6
Several determinations at 2^ and at 56^ are also given.
100 cc. anhydrous hydrazine dissolve i gm. KsCOs at room temp.
(Welsh anaBroderson, 1915.)
100 gms. aqueous solution simultaneously sat. with KiCOa and cane sugar at
31.25^ contain 22.24 %^'^' KiCOs and 56 gms. sugar. (K(}hler. 1897.)
Freezing-point data for mixtures of KsCOs + kCI and KsCOi + NaCl (Sackur,
1911-12). KiCOi -h KjSOi (Amadori, 1912; Le Chatelier, 1894); KsCOt
+NasCOs (Le Chatelier, 1894). (U Chatelier, 1894)
POTASSIUM Sodium CARBONATE K,COs.Na,CO,.i2HsO.
Solubility in Water at 25*.
Gnu. per loo Gnu. Sat. Sol.
(Osaka, z9zo-xx.)
Gnu. per too Gms. Sat. Sol.
K«CO,.
Na«CQ..
■N ooua riuuc. ^
KtCO,.
Na,CO».
•« ooua Tvmao,
52.83
0
K|COk.aHtO
25.2
14. 1
E«COk.NaiCQ,.zaB^
52
I
M
22.4
16.6
i«
50.7
2.6
M
19.8
18.7
«
49.1
4.6
" +K,(X\.Na,(X\.«H^
19. 1
19.7
(«
49
4.6
K,(X)k.Na,CQa.iaH,0
15 I
23.2
" +Na,COi.ioHiO
46.5
4.3
i<
14.5
22.8
NaiCO|.ioH/)
46.2
5-2
i«
10.8
22.7
(1
41
6.3
f(
10.7
22.4
ft
37.7
7
H
4.7
21.9
i(
31
10. s
If
0.
22.71
11
The previous determinations of Kremann and Zitek (1909), agree in general
with the above, but these authors report that the double salt contains 6H«0
instead of 12 HsO.
100 gms. HsO dissolve 184 gms. potassium sodium carbonate at i^ {d » 1.366).
(Stolba, 1865.)
POTASSIUM UBANTL CARBONATE 2K,C0s.(U0s)C0..
100 gms. HsO dissolve 7.4 gms. salt at 15^. (Ebelmen, xSsaO
POTASSIUM CHLORATE KCIO..
Solubility in Water.
Average curve from results of (3arlson (1910), Calxolari (191 a), and Tsdiugueff and CHUopb (1914).
f.
i of Sat. SoL
Gnu. KC10| per
zoo Gnu. H^.
0
1. 021
3-3
10
• • •
5
15
• • •
6.1
20
1.045
7-4
25
• • •
8.8
30
• ■ ■
10. 5
f.
i of Sat. Sol.
1.073
40
50
60 I. 115
80 I . 165
100 I. 219
104 b. pt. 1 . 230
For previous results in good agreement with the above, see next page.
Gnu. Ka^ per
too Gms. ^).
14
19.3
24.5
38.5
57
60
513
POTASSIUM CHLORATI
POTASSIUM CHLORATI KClOt. (See also previous page.)
SOLUBILITT IN WaTER.
(Gay-LttaBac, 18x9; Pawlewski, 1809; above zoo**, Tilden and Shenstone, z88z;'86e also Blaiei,
1891; Etard, 1894; at 99% Kfihler, 1879.)
Gma. KCIO; per 100 Gms.
Sdution. Water.
Solution.
70 22.55
80 26.97
90 31.36
IOC 35.83
120 42.4
136 49 • 7
190 64.6
330 96 -7
*Gay Lnaaac.
100 gms. HjO dissolve 5.06 gms. KClOa at lo**.
One liter of H2O dissolves 65.5 i^ms. KClOt at about 20
Gms. KC10» per 100 Gms.
Water.
1 A
0
3
04
314
3-3'
10
4-
27
4-45
50
20
6.
76
7.22
71
25
7-
56
8.17
8.6
30
8
.46
9.26
10. 1
40
II
•75
13-31
145
50
15
.18
17 -95
19.7
60
18
•97
23.42
26.0
29.16
36 -93
46.11
55 54
73-7
98.5
183.0
2930.00
32.5*
39-6
47-5
56.0
73-7
99.0
183.0
(Rooseboom, 189x0
^ ^ (KoDowalow, 1899b.)
One liter o\ 5.2 % NHi solution dissolves 52.5 gms. KClOi at about 20°. "
Solubility of Potassium Chlorate in Aqueous Solutions of Potassium
Hydroxide, Hydrogen Peroxide, and Mixtures of the Two at 25**.
(Calvert. 190Z.)
The mixtures were agitated by means of a stream of air. Equilibrium was
approached both from above and below 25**.
Mob. KGQi Gms. KClOk
Composition of Solvent. Dissolved per Dissolved per
Liter of Sat. SoL liter of Sat. Sol.
Water alone
0.67s
82.71
Aqueous 0. 125 n KOH
•
0.625
76.60
" 0.25 n " .
O.S73
70.23
Aq. HsQi containing
1.26
mols. HiOi per L
0.730
89.4s
(( «
I 31
0.737
90.33
Aq. 0.25 n KOH "
0.015
•*
0.578
70.82
u tt
0.276
0.584
71-57
It tt
0.9S4
0.616
75.50
tt tt
1.073
0.673
82.47
Solubility of Potassium Chlorate in
Aqueous Solutions
( OF
Potassium Bromide at 13''.
(Blarez
, 19x1.)
■-
Cms. per 100 Gms.
Solution.
Gms. per 100 Gms.
Solution.
Gms. per xoo
Solution
Gma.
•
'KBr. KQOj.
KBr.
Kaoj.'
KBr. KQCj.
0.20 5.18
I.O
5 04
6
•0 3
.46
0.60 5.20
2.0
460
8
.0 2
.80
0.8 5.06
30
40
4.2
40
10
.0 2
.40
Solubility of Potassium Chlorate in Aqueous Solutions of Other
Potassium Salts at 14^-15*. (Blarez, 19x1.)
Salt.
KOH
KCl
tt
KBr
tt
EI
it
Cms. per xoo Gms. Solution.
KSalt.
1-43
1. 91
3 82
3 05
6.10
425
8.51
KClOs.
4-47
4-45
3 58
4.49
3 60
4-59
3-65
Sdt.
KN03
tt
KjSO^
it
K3C3O4
Gms. per 100 Gms. Soltttloii.
((
KSalt.
2.59
518
2.23
4.46
2.42
4-85
KClOa.
451
3-88
4.71
3 98
4.7a
3-93
POTASSIUM GHLORATI
514
Solubility op Potassium Chlorate in Aqueous Solxttions of
Potassium Chloride at 20°.
(Winteler — Z. Electrocfaem. 7, 360, '00^
Sp. Or. of
SolutioDS.
1.050
I 050
1.050
I 054
1.064
1.086
Grams per Liter.
Kao^:
fa
o
10
20
40
60
80
100
71. 1
58 o
49.0
395
34 o
30. o
27.0
sp. Or. of
Soltttioos.
1.098
1. 108
1. 119
1. 130
1. 140
1. 168
fcT
120
140
160
180
200
250
Gnuns per liter.
Kao^:
245
22.5
21 .0
20.0
20.0
20.0
Solubility of Potassium Chlorate in Aqueous Solutions of
Potassium Nitrate.
(Arrhenius — Z. phyaik. Chem. ii» 307, '93.)
Results at 19.85^
Mdi. per Liter.
Grams
per Liter.
kNOs.
KClOj.
KNO,.
KQCi
0.0
0.570
0.0
69.88
0.125
0.529
12.65
64.86
0.25
0.492
25.29
60.33
z.o
0.374
IOI.I9
45-85
2.0
0.328
202.38
40.22
Results at 23.87
Mols. per Liter
' KNOi, KClOk
o-o 0.645
0.5 0.515
Grama per Liter.
KNOt. KCi^
0.0 79 09
50.59 63.14
S(h.ubility of Potassium Chlorate:
(Taylor, 1897; see also Gerardln, 1865.)
In Aqueous Alcohol.
At 30*.
I. KClOs
Wt. per cent ^
AlcoVolor Gma. KLlUi per
of Acetone lOo Gms.
insolvent. Solution.
O
5
10
20
30
40
50
60
70
80
90
923
7.72
6.44
4-51
3.21
2.35
1 .64
1 .01
0.54
0.24
0.06
Water.
10.17
8.80
7 65
5-90
4-74
4.00
3-33
2-53
1.82
1 .22
0.62
At 40'.
I. KClOa
Gma.
100 Gms.
per
Water.
In Aqueous Acetone.
At 30*.
Gms. KClOa per
ICO Gms
Solution.
12.23
10.48
8.84
6.40
4.67
3 41
2.41
1. 41
0.78
034
0.12
* Solvent, 9.09 Wt. per cent Acetone.
13 -93
9-
12.33
8.
10.77
7-
8.56
6.
7.00
4-
5-88
3-
4 94
2.
3 69
2.
2.63
I .
1-73
0.
1. 17
0.
At 40°.
Gms. KClOi
100 Gms.
tion.
Water.
Solution.
Water.
23
10.17
12. 23
13 -93
32
956
II .10
13. II
63*
9.09
10.28*
12.60
09
8.10
8.27
II .26
93
7.40
6.69
10. 24
90
6.76
5 36
9-45
90
5 98
4 03
8.40
03
517
2.86
7-35
24
4.18
1.68
5.68
57
2.88
0.79
3-97
18
1.82
0.24
2.45
100 gms. sat. solution of KClOi in glycol contain 0.9 gms. KClOa.
(de CooiDck, 1905.)
515
SoLUBiuTy OF Potassium Chlorate in
Compounds at 25**.
POTASSIUM CHLORATE
Aqueous Solutions of Various
(Rothmund, 1910.)
Aqueous 0.5 Normal
KClOi per Liter.
Aqueous 0.5 Normal
KClOb per Liter.
Solution of:
' Mob.
Cms.
Solution of:
Mols.
Cms.
Water alone
0.1475
20.44
Ammonia
0. 1474
20.43
Methyl Alcohol
Q. 1402
19- 43
Dimethylamine
0. 1342
18.60
Ethyl Alcohol
0. 1356
18.7s
Pyridine
0. 1410
19.54
Propyl Alcohol
0.1343
18.61
Urethan
0.1400
19.40
Tertiary Amyl Alcohol
0.1279
17.72
Formamide
O.IS39
21.32
Acetone
0. 1451
20.11
Acetiimide
0.1447
20.05
Ether
0. 1336
18.51
Acetic Acid
0. 1462
20.26
Glycol
0. I416
19.62
Phenol
0. 1362
18.87
Glycerol
0. 1404
19. 45
Methylal
0.1400
19.40
Urea
O.151O
20.92
Methyl Acetate
0. 1429
IQ.80
100 gms. glycerol (in= i .256) dissolve 3.54 gms. KClOtat 15-16®. (Ossendowski. 1907.)
POTASSIUM PerCHLORATB KCIO4.
Solubility in Water.
(Average curve from results of Noyes and Sammet (1903); Carlson (19x0); Rosenheim and Weinhaber
doi
Gms. KClOiper
xoo Gms. H^.
Sat. Sol.
0
1.007
0.7s
10
• • •
I OS
20
I. Oil
1.80
25
1. 012
2.08
30
• ■ •
2.6
40
1.022
4.4
v.
Sat. Sd.
59
60
• • •
70
80
• ■ •
I 053
90
■ • •
100
1.067
C^ms. Ka04
per
xoo. Gms.
Sat.
SoL
6
•s
9
II
.8
14
.8
18
21
.8
Solubility of Potassium Pbrchilorate in Aqueous and in Alcoholic
Solutions of Perchloric Acid at 25.2**.
(Thin and Cumming, 1915-)
In Aq. HCIO4 Solutions. In Alcoholic HCIO4 Solutions.
No™gmj,^af Ag. ,G«s._KaO,|» A.^cou. Solvit. .^-S;^.12.i3.
0 (= water) 2.085 93-5% Alcohol 0.051
o.oi 1-999 " +o.2%HC104* 0.0175
o. 10 1 . 485 98.8% Alcohol + " o . 010
1 0.527 " +2%HC104* 0.028
* The HQO4 was added as aq. 30% HCIO4 solution hence the concentration of the alcohol was decreased*
Solubility of Potassium Perchlorate in Aq. KCl and Aq. KtSOi
Solutions at 25**. (Npyes and Boggs, 1911.)
In Aq. KCl Solutions.
Gms. per loo.a cc. Sat. Sol. wt. of X00.2 cc
KCK)4.
2.0566
1.7800
1-5597
KCl.
O
O.371S
0.7421
of Solution.
• • •
101.42
101.45
In Aq. KsSOi Solutions.
Gms. per loo.a cc. Sat. Sol. wt. of ioo,a cc.
KCIO4.
2.0566
1.8262
I . 6396
K,S0«.
O
0.4339
0.8665
of Solution.
• • •
101.47
101.55
100 gms. 51.2 Vol. % Aq. CjHjOH (<i =0.9319) dissolve 0.754 em. KCIO* at 25.2*.
If
II
II
it
93.5
98.8
II
II
It
II
((^s 0.82 19}
(<i =0.7998)
90 Wt. % Aq. C,H,OH
97.2
u
l«
II
II
II
i*
and Cumming, 1915.)
0.051 em. KCIO4 at 25.2*.
(Inin and Cumming, x9X5-)
0.019 gni. KCIO4 at 25.2*.
(Thin and Cumming, X915.)
0.036 gm. KCIO4 at 25.2^
(Wenze, 1891.)
0.0156 gm. KCIO4 at 25.2*.
(Wense, 1891O
POTASSIUM CHLORIDB 516
POTASSIUM OHLOBIDB KCl.
Solubility in Water.
(Averace curve tram the Ktults of M
Ver. ZuckeriDd. 47. 447> '07; Andne —
W> 137. '6s; de Coppct IMd. [5] 3o» 4
andShcnrtonc ~ Proc. Roy. Soc. (Lobd
[cuMer — 2. anorc. Cb
-J. pr. Chem. [aj aOk
II. 'S3; EtMTd Ibld.ij]
•) 3& 345. '83.)
em. 44* V
456, *8^;
3,Sa6. '94
9* 05; at 31.3^1 K.oUer —
Gerardin — Ann. chim. idi
:t Mulder; above xoo°. Tile
^0 Cms. KCl per too Gnu.
^^ Gms.KClpo'tooGma.
^ ' Solution. Water.
► ••.
Gms.KQ per xoo Gms.
Solution.
Water.
'Solution. Water.
-9
19-3
239
40
28.6
40.0
147
41.5 708
-4-5
0
20 -6
21.6
25 -9
27.6
50
60
29.9
31 -3
42.6
45-5
180
43-7 775
Solid Phase Ice
5
22.7
29 -3
70
32.6
48.3
-9
193 23.9
10
23-7
31 0
80
33-8
511
-8.
17.7 21.5
IS
24 5
32 -4
90
351
54 0
-8
16.7 20.0
30
25-4
34 0
100
36.2
56.7
-7
14.9 17.5
35
26.2
35 5
130
39-8
66.0
-6
136 157
30
27.1
37 0
-5-5 ".5 14-3
±»
doi
Gms. KCl per 100
Gms. H9O.
f.
dci
m .
Sat. Sol.
Sat. Sol.
0.70
1.1540
28.29
74.80
1.2032
19 -55
I. 1738
34-37
89 -45
1.2069
32.80
I . 1839
3^-3^
108 (b. pt.)
I.2II8
59 85
I. 1980
45 M
Sp. Gr. of solution sat. at o — ^1.150; at 15® — 1.172.
The following determinations of the solubility of potassium chloride in water,
made with exceptional care, are reported by Berkeley (1904).
Gms. KOper 100
Gm8.H^.
49 58
53.38
58."
100 gms. H|0 dissolve 36.12 gms. KCl at 25^ (Amadoriand Pampanmi, 1911.)
F.-pt. data for aq. KCl solutions are given by RoIoflF (1895).
Data for equilibrium in the system potassium chloride, arsenic triozide and
water at 30** are given by Schreinemakers and de Baat (19 15).
Solubility of Potassium Chloride in Aqueous Solutions of Hydro-
chloric Acid at 0° and at 25°.
(AnnstroDg. Eyre. Husaey and Paddinson, 1907; Armstrong and Eyie. igxo-xx.)
Solvent,
Gms. HCl per
xooo Gms. H9O.
O
9. II
18.22
36.45
109 35
182.25
Solubility of Potassium Chloride in Aqueous Solutions of Hydro-
BROMic Acid and of Hydrochloric Acid at 25*^. (Hers, loxx-ia.)
In Aq. HBr. In Aq. HCl.
Millimols per xo cc. Gms. per Liter. Millimols per xo cc. Gms. per Liter.
Gms. KCI per
xoo Gms. Sat. Sol.
Ato*.
At as'.
22.11
26.45
20.93
25 17
19.71
24.07
17.26
21.74
. . •
13 -47
• ■ ■
6.93
HBr. KG. HBr. KCl. HCl. KCl. HCl. KCl.
o 42.72 o 318.5 5.66 37.49 20.64 279.6
6.61 37.80 53.5 281.9 10.20 33.79 37-19 252
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 17.39 118. 6 129.6
517
POTASSIUM CHLORIDE
Solubility op Potassium Chloride in Aqueous Solutions op
Hydrochloric Acid at o**.
Ueannel — Compt. rend. 103* 381, '86; Engel — Ann. chim. phys. [6] 13^ 377, *SS^
Milligram Mols. per 10 cc.
Grams per 100 cc. Solution, gp. Gr. of
KQ.
Ha:
K.CI.
HCI. Solutions.
34.5
0.0
25-73
0.0 ]
f-i59
30.41
3-9
22.69
1.42 ]
[.152
27-95
6.6
20.84
2.41 ]
M50
27-5
7-1
20.51
2.59 3
[.147
23-75
II. I
17.71
4.05 ]
t-137
16.0
23-0
"•93
8.39 3
:.iii
10. 0
34 -o
7.46
12.40 ]
[.105
7-5
41.0
5.60
14-95 3
[.los
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. KCI at 17*^. (Ditte, i88x.)
100 gms. sat. aq. HCI solution dissolve 1.9 gms. KCI at 20^. (Stoltsenbeis, 191a.)
F.-pt. data for mixtures of KCI and HCI are given by Demby (1918).
Solubility of Mixtures of Potassium Chloride and of Sodium Chloride
IN Aqueous Hydrochloric Acid Solutions at 25".
(Hicks, 19x5.)
Gms. per 100 Gms. Sat. Solutions.
' HCl.
NaCl.
KCI.
0
19-95
10.90
8.61
10.65
7.58
17.16
356
3-8o
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, '8x.)
Grams KCl
per TOO Grams Sat. i
Solution in:
f.
MVcia.
14-3
9-9
21.2%
MgCia.
5-3
1.9
>o%M((a,.
10
4.2
KCI+S.7]
STaC
20
15-9
"•3
6.5
2.6
6.0
" +5-9
30
17-5
12.7
7.6
3-4
6.9
" +6.0
40
19.0
14.2
8.8
4.2
7-9
" +6.1
50
20.5
15.6
10. 0
5-0
8.9
" +6.3
60
21.9
17.0
II. 2
5.8
9.9
" +6.4
80
245
19-S
13.6
7-3
10.9
" +6.6
90
25.8
20.8
14.7
8.1
II. 9
" +6.7
t(
100
27.1
22.1
15-9
8.9
13 0
" +6.9
a
More recent data on the solubility of potassium chloride, in aqueous solutions
of magnesium chloride are given by Feit and Przibylla (1909).
POTASSIUM CHLORP>B
518
SoLUBn^iTT OF Mixtures of Potassium Chloridb and Potassium
Bromide at 25**.
(Fock, 1897.)
Gnmsper liter
SolutioD.
MnUgrmmMob.
per Liter.
Mol. percent
KClin ,
SoluUon.
Sp.Gr.of
SolutioDi.
Mol. per cent
KOin
K.Br.
KQ.
KBr.
KCl.
Solid Phase.
558 I
0.00
4686.2
0.0
00 1
^•3756
0.00
5315
23 -44
4462.7
3M-2
6.16 1
[.3700
0.00
503-6
46-57
4228.5
624.3
12.86 ]
[.3648
8.23
454-6
82.62
3817.8
II08.O
22.49 3
1-3544
15-68
379-6
136.6
3188. I
1830.7
36.48 ]
f-332o
33-66
324 8
166.9
2727.6
2237.4
45.06 ]
[.3119
63 51
2x8. 0
213.9
1830.2
2868.0
60. 30 1
[.2689
82.29
140.7
250.9
I181.I
3363-9
74.01 ]
1-2455
88.04
47 -S
291.7
398 -8
39" -4
85.22 ]
[.1977
96.98
0.0
3"-3
00
41731
100. 00 :
[.1756
100.00
Solubility of Potassium Chloride in Aqueous Potassium
Hydroxide Solutions.
(Engel — Bull. aoc. chim. [3] 6» 16, V. Winteler — - Z. Electrochem. 7, 360. '00.)
Results at <
0**.
Results at 20
•
•
(Engel.)
(Wintder.)
Mg. Mo
xo cc. S(
Is. per
llUtlOD
KOH.
Sp. Or. of
Solutioa.
Gnu. per 100 cc.
SofutioD.
KCl. KOii.
Gins, per 100 cc. _ _ ,
Sokitioo. Sp. Gr. of
ka. 'koh.- ^'^^
Ka.
35-5
0
I 159
26.83
0.0
29 3
I.O I
.185
31.0
2.375
1. 146
23-44
1-33
21. 1
10. 0 I
310
28.3
4.7
I -153
21-39
2. 64
14.8
20.0 I.
245
23.0
9.9
1. 172
17-39
5 56
10.4
30.0 I
29s
18.38
15 I
I -195
13.89
8.46
6.8
40.0 I
34S
14-43
20.0
1. 216
10.91
11.23
4.0
50.0 I
397
"-43
24.63
1-239
8.64
13 83
2.2
60.0 I
4SO
8.98
29.25
1. 261
6.78
16.43
1.4
70.0 I
Soo
6.28
35-^3
1.294
4-74
19.72
i.i
0.9
80 0 I
85.0 I
SSO
.580
Solubility of Mixtures of Potassium Chloride and Potassium
Iodide in Water.
(Etard — Ann. chim. phys. [7] 3, 275, '94.)
Gnnu per
TOO Gms. Solution.
AO
Grams per
100 Gms. Solutian.
• •.
KCl.
Kl.
t .
KCl.
KI.
0
3-7
50-5
100
6.2
61.0
20
4-2
53 0
140
7-3
63 -7
40
4-7
55-3
180
8.3
6SS
60
S-a
57-5
220
9.4
66.3
80
5-7
59-4
245
10. 0
66.5
519
POTASSIUM CHLORIDE
SOLUBILITT OF POTASSIUM CHLORIDE IN AQUBOUS SOLUTIONS OF POTASSIUM
Iodide at 25** and Vice Versa.
(Amadori and Pampanini, 191 z.)
Gms. per zoo Gms. HjO.
Cms. per zoo Gms. HfO.
KG.
KI. '
KQ.
Kl.
0
149.26
19.64
68.22
4.06
144.03
23-75
4389
763
137-79
29.56
23-^3
11.36
132.60
31-38
14.83
11.74
133 90
33-68 •
7
15.10
105.91
36.12
0
Solubility of Potassium Chloride in Aqueous Solutions of Potassium
Nitrate at o® and at 25®.
(Armstioog and Eyre, zgzo-zz.)
Sohrent, Gms. KNOk
per zoooGms.
O
25.27
50.55
lOI.II
151.66
Gms. KQ Dissolved per
zoo Gms. Sat. Solution at:
o".
22.10
21.71
21.25
20.70
25"'
26.73
26.26
25.61
24.58
23 -57
Solubility Data for the REapROCAL Salt Pairs KCl+NaNOti=fcNaCl+KNOi
AT 5°, 25^ 50® AND 100**.
(Reinders, Z9Z4, Z9Z5; see also Uyeda, Z909-Z0.)
Results at 25®.
Gms. per zoo Gms. H|0.
NaQ.
36.04
32.28
30.27
12
10
23.62
33.90
24.82
21.36
24. s
7
23.8
4.5
KCl. NaNQi. KNO,.
10
16
26
35
34
10
22
20
45
78
54
92
xo
60
100.9
0.o6
77.46
58.01
10
15.4
• • •
61.3
82.1
64
Results at 5*.
31.50 10.4
29.84
■ • • • • •
27.6
10
22
31
37
41
46.
20
32
17
43
41
40
10.14
82.10 18. 1
41.7
Results at 50^.
Gms. per zoo Gms. ^O.
NaCl.
KCl. NaNQ.. KNQ..
a ■
36.72
■ • •
■ •
• •
• ■
28.35
• • •
23.09
• •
• •
• •
42.80
41.39
• •
24.
.79
38.75
52.
■48
85.
.49
• •
.87
• •
.15
134.9
114. 1
90.
• •
• ■
20. s
84.8
• •
« ■
28.4
43-9
• ■
• •
34
13.4
• • •
»4-
.9
12.7
25.4
• ■ ■
S8.
.2
« • •
• • •
• ■ a
■ ■
.15
19.2
• • •
104. 1
27.
.2
12.2
• • •
IIO.7
82.
.3
59.9
■ • •
6.1
70.
05
54
10
3
6
2
2
9
Results at Ioo^
27.3 36.2
... 41.6 ... 199
233.6 218
19.2 ... 158
SoUd Phase in Each
Case.
NaQ
((
NaQ+Ka
KG
(I
KQ+KNQ.
KNQi
<(
tt
KNQi+NaNQi
NaNQi
NaNQa+NaQ
Naa
NaCl+KQ
KQ+KNQ,
KNOa+NaNQ,
NaN0,+Naa
Naa+NaNQ,+KNQi
NaQ+KCl+KNO,
NaQ+Ka
KQ+KNQi
KNOi+NaNQi
NaNQ,+NaQ
POTASSIUM CHLORIDB
520
SOLUBILITT OF POTASSIUM CHLORIDE IN AqUBOUS SOLUTIONS OF POTASSIUlf
Nitrate, and of Potassium Nitrate in Aqueous Solutions of Potassium
Chloride, at Several Temperatures.
(Touren. 1900; BodULnder. 1891; Nkot, 1891; Soch, 1898.)
KCl in Aq. KNOi Sc^utions at:
I4.5'
(T.).
25.2*
(T.).
20*, etc. (N.).
Gnu. per Liter Solution.
Gms. per Liter Solution.
Gms. per xooo Gms. S^O.
KNOb.
KCL
KNOb.
KCl.
KNOb. KO.
0
288.3
0
3". 8
0 345-2
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 s
122.7
287.2
225.8 341.3
"5-9
270.7
141. 4
284.2
at 80** (S)
119. 1
268.3
182.7
276
II7S 402
123.4
267.2
KNOi in Aq. KCl Solutions at:
*
14.5*.
25.
2».
20«.
Gnu. per Liter Solation.
Gms. per Liter Solution.
Gms. per xooo Gms. H^O.
KCL
O
13.58
31 63
65.64
132.6
164.4
196.5
236.9
KNObT
225.4
219.8
208.2
185.2
159 5
153-3
144
137 -I
KCL
O
19-39
49.22
100.7
155-2
207.3
226.8
KNOb.
325-5
312.3
288.7
254
224.4
203.9
196.9
KCL
O
82.9
165.8
248.7
3108
KNOb.
311. 1
256.8
221.7
202
501.6
In the case of the results by Touren, constant temperature and agitation were
employed.
KNO, in Aq. KCl at 20.5^ (B.).
KCl in Aq. KNQi at 17.5" (B.).
3ms. per xoo oc
Solution.
Sp. Gr. of
KCL
KNO,.
Solutions.
0
27 68
1. 1625
4-72
24.39
I. 1700
7-74
22.44
1. 1765
12.23
20.23
I . 1895
15.15
18.96
I . 1983
19.61
17.67
1. 2150
22.17
17. II
1.2265
24.96
16.79
1.2400
Gms. per xoo oc
. Solution.
Sp. Gr. of
KNOb.
KCL
Solutions.
0
29-39
1. 1730
6.58
27.50
. 1. 1980
8.88
27.34
I. 2100
12.48
26.53
1.2250
14-83
25.98
1.2360
15.22
25.96
1.2390
15-49
25-95
1.2388
15-33
26.24
I . 2410
In the case of the above results by Bodl&nder, a saturated aqueous solution of
potassium chloride was prepared and weighed amounts of potassium nitrate weve
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
Sqlubility of Potassium Chloride in Aqueous Solutions of Potassium
Nitrate and Vice Versa.
(Leather and Mukcrji, 19x3.)
Results at 30^. Results at 40"*. Results at 91^.
Sp.Gr. ^°"- P^JS^ ^"'- Sp. Gr. ^™P^~^°^- Sp.Gr. ^""P^^^"^ Solid Phaae
^^•^** KCl. 'kNQ.; ^^•^' KQ. KNQ,; ^'^^- ' KO, ' KNO,.' Each Case.
1. 186 37.58 o I-I94 40.60 o 1.222 53.58 O KQ
I.2I9 36.72 8.05 1.252 39.11 16.86 1.344 47.85 52.75
I.25I 36.19 19.36 1.305 37.08 35.45 1.486 43.30 II4.6
I.281 35.42 26.83 I.319 37.49 39.71 1.552 39.90 162.9 " +KNQ,
1.258 28.71 29.19 I.312 32.22 41.52 1.544 33.25 165.6 KNQ,
1.241 19-35 32.34 1-297 22.63 46.31 1.545 15-56 181. 1
1.225 9.44 38.10 1.279 11.58 52.66 1.552 o 202.8
Results are also given for 20^.
Solubility of Mixtures of Potassium Chloride and Sodium
Chloride in Water.
u
tt
If
f.
Gms. per xoo
Gms. HiO.
f.
Gms. per xoo Gms. H|0.
KQ.
NaQ.
KCl. NaCL
0
11.2(1) 11.2(2) 30(1) 30(2)
50
22(1) 19(2) 27.7(1) 32.3(2)
10
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
17.1(3) 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
(x) Precht and Wittgen, i88z; (3) Etard, 1897; (3) at 35" 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.)
Results at 20"*.
Results at 40^.
>
Results at 91*.
Sp. Gr.
Sat. Sol.
Gms. per 100 Gms.
HA
Sp. Gr.
Sat. Sol.
Gms. per xoo Gms.
H;0.
Sp. Gr.
Sat. Sol.
Gms. per xoo Gms.
H«0.
SoUd Phase
in
KQ. NaQ.
KCl. NaCl. '
KQ. NaQ.*
Each Case.
1. 176
34.61 0
1. 194
40.60 0
1.222
53.58 0
KQ
1. 197
26.60 10.13
1.207
31.42 10.68
1.236
45.01 10.66
<f
I.213
19.65 20.61
1-235
24.43 20.99
1.262
35.84 22.87
i(
1.237
14.92 30.36
1.248
18.23 30.60
1.262
33.12 28.12
M
1.240
15.36 29.61
1.242
18.74 30.32
1.264
32.45 28.26
" +Naa
1.233
14.76 30.38
1.247
19.13 .29.92
1.235
27.15 29.18
NaQ
1.224
9.70 32.40
1.222
10.49 32.59
1.223
13 33.93
«
I.193
0 35-63
I.I97
0 36.53
1. 189
0 38.72
M
Results are also given for 30**.
100 gms. 40 wt. per cent alcohol dissolve 5.87 gms. KCl + 12.25 fi^s. NaCI at 25".
100 gms. 40 wt.'per cent alcohol dissolve 5.29 gms. KNOt + 10.06 gms. KCl at 25^.
(Soch, 1898.)
100 gms. abs. ethyl alcohol dissolve 0.034 S™* ^^^ ^t 18.5^.
100 gms. abs. methyl alcohol dissolve 0.5 gm. KCl at 18.5^
(de Bniyn, x89s; Rohland, 1898.)
POTASSIUM CHLORIDB 522
Solubility Data for thb Reciprocal Salt Pairs KCl+NaiS049dbKiS04+NaCl.
(Meyeriioffer and Saunden, 1899.)
J nt Molt, per xooo Molt. H^.
f. . "k^^ t • * Solid Phase.
Sat. Sol. S0«. K«. Nat. CI,.
4.4* ... 5.42 14.39 5183 60.8 K,Na(S04)t+KCl+Naa
0.2 ... 3.3s 12. 7« 50.93 60.36 Na«S0«.xoH«0+Ka+Naa
— 0.4 ... 3.59 16.38 40.75 53.54 Ka,S0«.xoH/)+Ka+K,Na(S04),
16 ... 472 1758 5056 63.42 K.Na(S04)s+Ka+Naa
24.8 X.2484 4.37 20.02 48.36 64.01 "
16.3* ... 16.29 9.16 61.06 53.93 K,Na(S04)s+Naa+Na«S04.ioR^+Na«SO«
24.5 1.2625 1445 9 90 58-46 53-91 K,Na(S04),+Naa-hN«,S04
0.3 •• 2-75 25.77 17.93 40.9s K,Na(S04),+Ka+K,S04
25 X.2034 2.94 36.20 14.80 48.06 "
17.9* 1.2470 13.84 O 62.54 48.70 NatSO«.xoR^+Na«SQ|+Naa
30.1* 1.289 SO. 41 10.08 40.33 O K.Na(S0J,+Na,S0«.xoH/)+Na,S0«
• 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.
^ Gma. per 100 Gms. H/). ^. „ Gins, per 100 Gms. HwO. ^.
•^' ' — ^t:; — :* — „ ^^ > Observer. «•. "^^
KQ + K«S04.
10 30.9 1.32 (Precht & Wttgen.) 40
15.8 28 2.3 (Kopp.) 50
20 33.4 1.43 (P. andW.) 60
25 34*76 2.93 (Van't Hoff & Meyerhoffer.) 80
30 36.1 1.57 (P.andW.) 100
ICO gms. aq. solution, sat. with both salts, contain 26.2 gms. KCl + 1.09 gms.
KsSOi at 30^. (Schreinemaken and de Baat, X914.)
S(H«UBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS 'OF STANNOUS
Chloride at 25* and Vice Versa. (Fujimura, 19x4.)
Gms. per 100 Gms. H/). ^ .. . . Gms. per 100 Gms. H«0. ^ ,. ^ ^.^
O 34-73 ^° 58.48 17-85 Sndt-KdHW
KQ
+ K^4.
38.7
1.68 (P.andW.)
41 -3
1.82
43-8
1.94
49.2
2.21
54.5
.2-53
M
11
If
11
M
2.86 32.17 " 81.78 19.06
4.37 34.08 •; 107.65 17.79
S-9S 31-76 SnCU.aKa.aH,0 170.70 21.26
5.83 30.65 " 247.50 24.38
10.24 27.30 " 337 26 25.51
17.42 24.68 " 290.30 19.66 SnCU.jH^
27.88 24.40 " 235.50 7.49
34.28 5.99 " 222.5 2.73
54 .19 19 . 45 SnOi-KCLEdO 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, 19x0-11.)
C^0&
Gms. KG]
Dissolved per xoo Gms.
Sat. Sol. at:
rf|.o£
SoLSat.
I.1813
m
Solvent.
0
22.1
as'.
26.44
1. 14
2.25
4.41
8.44
21.6
20.9
19.7
• • •
25-91
25.29
24.21
22.46
I. 1754
I . 1689
I. 1568
I. 1357
12.13
18.69
• • •
• . .
17.42
• . .
1.0847
523
POTASSIUM CHLOUDB
Solubility op PoTitssiuM Chloride in Aqueous Alcohol.
(Gerardin -^ Ann. diim. phys. [4] & i40» '65.)
Interpolated from the original results.
Grams KCl per xoo Cms. Aq. Alcohol of Sp. Gr.:
t«.
0.9904
wt.^4.
0^48
wt'f.
0.9793
-13^
Wt.%.
0.9726
— 19.1
Wt.%.
o^)S73
■■ 30
Wt.%.
o^)39
— 40
Wt.%.
0.8967
-60
Wt.%.
0.8244
— 90
Wt.%.
0
5
23 -4
2S.O
I9S
21.0
^5S
16.8
"S
X2.8
70
8.0
4.0
4.8
1-7
2.2
0.0
0.0
10
26.4
22.5
18.0
14.0
9.0
S-6
2.7
0.0
IS
26.8
24.0
19.2
^S'^
10. 0
6.4
31
0.04
20
29.1
2S-3
20.3
16. 1
10.8
7.2
35
0.06
2S
30 -4
26.8
21. s
17. 1
II. 6
7-9
3-9
0.08
30
31 7
28.0
22.6
18.2
12. s
8.S
4.2
o.io
40
34-3
30.8
24.8
20.0
14.0
9.9
4.8
0.20
SO
60
37 0
• • •
33 S
• • •
27.0
• • •
21.8
• • •
15s
16.8
10.8
II. 8
5-2
5S
0.30
0.40
Solubility op Potassium Chloride in Aqueous Alcohol at:
IS".
(Schiff — liebig's Ann. zx8» 365. *6i.)
Sp. Gr.
of
Alcohol.
Wt.
cent
G.Ka
xoo g. Aq
AJcohol.
0.984 10
0.972 20
0.958 30
0940 40
0.918 50
0.896 60
0.848 80
Gerardin 's results at 15° agree
well with the above deter-
minations.
;ipcr
_. Aq.
Alcohol.
19.8
14.7
10.7
7-7
50
2.8
045
14.5. .
(Bodl&nder — Z. physik. Ch. 7f 3z6i '91 •)
Sp. Gr.
of Sat.
Solutions.
I. 1720
1.1542
I • 1365
I.I07S
I. 1085
I 0545
I 0455
09695
0.931S
0.8448
Grams per igo cc. SolntJoo.
CsHftOH. H^O
2
4
10
15
20
24
40
48
68
• •
88.
•79
85 •
.98
84.
•56
79 •
•57
75 •
.66
70.
■25
67.
•42
50-
•73
40.
•63
IS-
10
78
00
63
24
52
OS
18
60
SS
29.10
26.85
24.67
20.56
17.24
14.27
13-25
6.3s
3 82
0.30
30° and 40**.
(Bathrick — J. Physic. Chem. z. 160, '96.)
Wt.
per cent
Alcohol.
Gms. KCl
Aq.
per xoo Gi
Alcohol.
At 30^
At 40**.'
0
38 -9
41.8
5.28
33-9
35-9
9-43
30. 2
33-3
16.9
24.9
27.6
251
19?
21.8
341
15 -6
17.2
Wt.
per cent
Alcohol.
43 I
SS-9
65 -9
78.1
86.2
Gma. KCl per xoo Gmt.
Uiper
Aq. Alcohd.
At3o*'.
ZI.I
6.8
3.6
1-3
0.4
At 40*.
13. 1
8.2
4.1
1.6
0.5
o
Mols.Ka
per Liter.
4.18
Gii».Kaper
100 oc. Sat. SoL
31.18
Wt.%
CAOH.
60
lO
20
3"
2.40
23 -93
17.89
70
80
30
1.78
13 27
90
40
so
1.26
0.84
9.40
6.26
100
POTASSIUM CHLOUDB 524
Solubility of Potassium Chloridb in Aqueous Solutions of Ethtl
Alcohol at 25**.
(Mcintosh, 1903.)
Mob. KQ Gm. KQ per
per Liter. loo oc Sat. SoL
0.56 4.18
0.30s 2.27
O.I2S 0.93
0.042 0.31
o.oii 0.08
Solubility of Potassium Chloride in Dilute Aqueous Solutions of
Methyl Alcohol at o® and at 25®.
(Armstzong and Eyre, 1910-1 z.)
Wt % Cms. KO per zoo Gnu. Sat. Sol. at:
Ci^H t * s
in Solvent. o*. 35*.
o 22.06 26.69
0.79 21.74 26.42
1.57 21.39 26.01
3.10 20.61 25.25
8.76 17-84 22.82
Solubility of Potassium Chloride in Aqueous Methyl Alcohol at 25^
(Hen and Anders, Z907; Mclntoeh, Z903.)
So^cPt. ^ ^ Gms-Ka Solvent. . ^ Gms.KQ
*'«f CH^H. Sat. Sol. Sat. Sol. «y CH/)H. Sat. Sol. Sat.SoL
0.9971 o 1. 1782 31.13 0.8820 64 0.9064 3.44
0.9791 10.6 1. 125 24.53 0.8489 78.1 0.8607 z>54
0.9481 30.8 1.033 13.65 0.8167 98. 9(?) 0.8242 0.7s
0.9180 47.1 0.9679 7.61 0.7882 100 0.7937 0.43
100 gms. methyl alcohol dissolve 0.53 gm. KCl at 25^. (Tuner and Biasett, X913O
ethyl " " 0.022 " "
propyl " " 0.004 " "
amy! " " 0.0008 " " "
Potassium chloride is insoluble in CHtOH at the crit. temp. (C^entnenxwer, 19x0.)
Solubility of Potassium Chloride in Dilute Aqueous Solutions of
Propyl Alcohol at o® and at 25®.
(Armstzong and Eyre, z9zo-xx.)
Wt.% Gms. KQ per zoo Gms. Sat. Sol. at:
tSif^ t • ^
in Solvent. o*. 25*.
I 22.06 26.44
1.48 21.25 25.94
2.91 20.49 25.23
5.66 18.97 23.82
Solubility of Potassium Chloride in Aqueous Solutions of Glucose at 25*.
(Armstrong and Eyre, z9io-zz.)
Wt. % Gms. KG
C|H|A+Ht0 per zoo Oto^
in Aq. Solvent. Sat. Solution.
o 26.63
4.72 25.86
9 25.18
16.53 23.89
37 27 20.15
5^5
POTASSITTM CHLORIDE
S(X.UBILITY OF POTASSIUII ChLORIDB IN AqUBOUS AcBTONB SOLUTIONS.
(Sndl, X898; at ao*, Hen and Knoch, X904-)
Wt. (see Note) At
«>•.
At
so*.
At4o'.
^ At so-.
Percent
Acetone in
KCl per xoo oc
SoluUon.
Cms. per xoo Gms.
Solution.
Acetone. KG.
Gms. per xoo Gma.
Solution.
Gms. per xoo Gms.
Solution.
Solvent.
lifllUimoIs.
Gm».'
Acetone. KCl. '
Acetone. KCl. '
0
410. s
30.62
0
27.27
0 28.69
0 30
9.1
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. s
12.42
35 52
II. 31
tt
36.03 9.93
SO
iiS-4
8.61
45 98
8.04
u
46.46 7.07
60
71.2
5 3^
56.91
5-1?
it
57-37 4.38
70
38-5
2.87
68.18
2.60
u
68.56 2.22
80
12.9
0.96
79-43
0.76
79-34 0.58
79.25 0.94
90
2
o.is
89.88
0.13
89.84 0.16
±81'' sat. sol.
100
0
0
100
0
100 0
Note. — For the 20® results the per cent acetone in the solvent b 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 80 Per cent the Saturated Solution Separates into Two Layers
Having the Following Compositions:
Upper Layer.
■
Lower I^yer.
Gms.
per xoo Gms. Solution.
Gms.
per xoo Gms. Solution.
' H/).
(CH^iCO.
KQ.
HiO.
{CH,),CO.
KQ.
55.2
31-82
"-99
28.14
69.42
2.44
53.27
35-44
11.29
30.96
65-97
3
,07
51.23
48.50
10.27
32.64
63-79
3
56
50.34
39-88
9-77
34.07
62.01
3
,92
48.02
43-18
8.79
37.44
57-67
4
.89
46.49
45-34
8.17
38.68
56-17
5
25
58.99
25-24
15-77
23.66
74-91
I.
43
100 cc. sat. solution of potassium chloride in furfurol (CiHsO.COH) contain
0.085 gm. KCl at 25^ (Waklen, 1906.)
POTASSIUM CHLOUDB
526
Solubility of Potassium Chloride in Aqueous Solutions of Glycerol at 25^
(Hen and Knoch, 1905.)
Sp. Gr. of Glycerol at 25"/4" - 1.2555.
Wt. Per cent
Gt^oerol in
Solvent.
O
13-28
25.98
45 36
KQ per zoo oc.
Solution.
MiUimob.
Gms.
424 s
383-4
31.66
28.61
339-3
25-31
271.4
20.24
Sp. Gr. of
Solutions.
1. 180
1.185
1. 194
1. 211
Impurity about 1.5%.
Wt. Per cent
GWctaA in
Solvent.
54.23
83.84
100
KCl per 100 CO.
Solution.
Millimols.
238. s
149
110. 6
Gms.
17.79
II. II
8.25
Sp.Gr. of
Solutions.
1. 219
1-259
1.286
100 gms. HtO dissolve 246.5 gms. sugar + 44.8 gms. KCl at 31. 25^ or 100 gms.
of the sat. solution contain 62.28 gms. sugar + ii*33 gms. KCl. (Kdhkr, 1897.)
Solubility of Potassium Chloride in Aqueous Solutions of Pyridine at io^
(Schroeder, 2908.)
Aq. Miztuie.
Gms. KCl
per 100 Gms.
Sat. Sol.
Aq. Blixture.
Gms.Ka
per xooGms.
Sat.SoL
ccHdO.
OC Pyridine.
be H^. oc Pyridine!
100
80
0
10
20
23-79
19.76
16.37
40 60
30 70
20 80
3-33
I-2S
0.24
70
60
30
40
13-19
10.05
ID 90
0 100
0.04
0
SO
SO
6.34
Solubility of Potassium Chloride in Dilute Aqueous Solutions of
Several Compounds at 25®.
(Armstioiuc and Eyie, 1913.)
Compound.
Water alone
Acetaldehyde
Paraldehyde
Glycerol
100
Gms. Cmpd.
per 1000 Gms.
II. 01
II. 01
13-01
Gms. KCl
per xoo Gms.
Sat. SoL
26.89
27.05
26.42
25-58
Gms. Cmpd. Gms. KCl
Compound, per xooo Gms. per 100 GmSi
Glycol
u
Mannitol
H«0.
15.51
62.05
45-53
136.59
Sat. SoL
26.43
25.26
24.86
24.46
fi^ms. 95% formic acid
" glycerol (du = i .256)
dissolve 19.4 gms. KCl at 19.7^. (Ascfaan, 19x30
3.72 " " " I5-I6'. (OMendowski, 1907O
n
fl
<f
100 cc. anhydrous hydrazine " 9 " " " room temp.
(Welsh and Broderson, 19x5.)
100 gms. hydroxylamine
If
12.3
if
ft
(i
17-18^ (de Bruyn. X893.)
Fusion-point Data (Solubilities, see footnote, p. i) Are Given for the
Following Mixtures of Potassium Chloride and Other Salts.
Kd4-KI i (^'■esnewski.'xa; Amadori&Pam- ir pi 4.1^.0(3 ( (Jaenecke, 'xs; Sackur, 'xx-is;
* ] panini, '11; Ruff & Plato, '03.) -r'vio'^i. J ^^ ^ Plato, '03.)
KCl +KF. (Ruff and Plato. X903.) KCl -f HgCl (Sackur. X913.)
KCl+KOH. (Scarpa, X9X5.) KCl+NaCl. (Sackur, '13; Ruff & Plato. 03.)
KCl+KCrOi. (Sackur, 'ix-x2;Zemcaizny, '08.) KCl+NasSOi. (Su^ur, 19x3.)
KCl+KPOt. (Amadori, X9xa.) KCl+SrCls. (Vortisch, '14; Sackur, 'xi-xa^
KCI+K4PSO7. " KCl+TlCl. (Sandonnini, 19x1: 1914)
KCH-K,P04.
M
POTASSIUM CHLOROmiDATE KsIrCU.
100 gms. HiO dissolve 1.25 gms. of the salt at l8-20^
100 gms. HiO dissolve 9.18 gms. dipotassium aquopentachloroiridite, IrCU
(HsO)Kt at 19"*. (DeMne. 1908.)
527
POTASSIUM CHBOMATBS
POTASSIUM CHBOMATES KsCrOi, KsCrsO?, KsCr,Oio, etc.
Equilibrium in the System, Potassium Oxide, Chromic Acid and
Water at Several Temperatures.
(Koppd and Blumenthal, 1907.)
Results at o^
Results
at 30^
Results at 6o*.
Gms. per xoo
Gms. Sat.
Gmt.per xoc
> Gms. Sat.
Gms. per zoo Gms. Sat.
Solution.
Solution.
Solution.
Sdid Phase at eadi
Temp.
K^.
CiOb. '
K^.
CiOi.
K^.
CrA.
31.18
...
46.8
• • •
about 50
• • •
K0H.3H«0
26.06
0.54
26.89
0.94
32.98
0.53
KtCi04
19.31
4.27
22.25
3.06
21.05
9.15
It
17.06
11.77
18.65
13-72
20.25
14.43
M
17.62
18.71
19.12
20.30
20.70
21.97
II
17.73
19.04
19.35
21
20.61
23.61
" +K,CrA
10.90
"•93
15.04
16.85
14.53
20.82
K,CrA
1.87
3.13
11.20
13. II
10.01
21.21
II
0.78
22.38
2.42
28.21
6.86
39.64
It
1.47
42.95
2.50
44.50
7.06
49.84
" +K,CrAi
1. 25
4452
• ■ •
• • •
4.06
54.73
KtCrAi
1. 17
46.84
• • •
• • •
2
60.69
II
1.37
47.40
2-35
49-95
• » •
•
• • «
" +K,Cr4Qu
1.24
48.23
I -35
53-39
• • •
• • •
CflCrAs
1. 16
56.93
• • •
■ • •
• • «
• • •
II
0.64
61.79
0.69
62.81
1.27
65.77
" +C1Q,
0
61.54
• • •
62.52
0
65.12
CiQ,
The Cryohydrates (Eutectics) in the System KjO — CrOi — H|0.
The points were determined by adding to a sat. solution of K2Crs07 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 CrOs
goes into the solid phase. This relation also holds at the points where the solu-
tion is simultaneously saturated with KiCrsO? and KiCrjOio or KaCrtOio and
KiCriOii.
r of Equi-
Gms. per zoo Gms.
SoUd Phase
r of Equi-
Gms. per
xoo Gms.
Solid Phase
librium of
Sat. Sol.
with Ice.
Sat. Solution.
in Equilibrium
with Sat. SoL
and Ice.
librium of
Sat. Sol.
with Ice.
Sat. Solution.
in Equilibrium
with <>ftt Snl
KA CiQi.
K/).
CrO».
WllU i3ikl. out.
and Ice.
-25
20 5.70
K<Cx0«
-13.22
not det.
27.26
K«CrA
-13
17.52 13.89
II
-14.50
«
28.85
II
-".37
17.12 18.18
II •
— 22.10
ti
35.92
II
-11.50
17.18 18. II
" +K,CrA
— 22.11
0.47
36.14
ii
•
-s
8.27 8.01
K,CrA
— 26.77
0.88
39-86
11
-0.63
1.38 2.93
II •
— 30.20
1. 18
42.31
" +K,Cr,0»
-1.78
notdet. 6.81
II
-34.01
0.95
43-45
K«CrA«
-55
" 16.05
II
-39
0.79
45.65
" +K,Cr4Qu
-6.43
0.48 17.25
II
-49
not det.
49.11
K«CrAi
10.25
0.45 23.63
II
-61.5
0.61
53.57
It
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 CrOi content is 59 gms. per 100 gms. sat. solution.
If
u
M
POTASSIUM CHBOHATBS 528
By interpolation from the data given in the preceding tables the following
solubilities in water are obtained:
The Ice Curve and SoLusn^iTT of Potassium Chrouate in Water.
— 0.99 4.53 Ice — 11.3s Eutec. S4S4 Icc+k^CiO*
— 1.2 6.12 " o 57-11 e«Ce0«
— 4.3 26.99 " 30 65.13
— 7.12 42.04 " 60 74.60
— 10.3s 52-41 " ios.8b.pt. 88.8
Potassium Potassium Dichromate Potassium Dichromate
Dichromate + Potassium Chromate. + Potassium Trichromate.
t*. perxooGms. t\ . — =r^ — * — - - > f. Solution.
IV). K^. CrOi. K/). CiQi.
—0.63* 4. SO — ii.s* 17.18 18. II —30* 1. 18 42. SI
o 4.65 o 17.73 19.03 o 1.47 42.99
30 18.13 +30 19.3s 21 +20 2.20 43.10
60 45-44 60 20.61 23.61 30 2.50 44.50
104. 8t 108.2 106. 8t 24.3 30. s 60 7.06 49.84
ii4t 16.80 59.20
* Eutec. t b. pt.
Potassium Trichromate -f- Potassium Potassium Tetrachromate+
Tetrachromate. Chromic Acid (CrOt).
Gnu, per 100 Gms. Sat. Sol. Gms. per xoo Gma. Sat. Sol.
"kJo! * CiQi. "kA * CiO*.
—39 Eutec. 0.79 45.69 o 0.64 61.79
o 1.37 47.40 20 0.62 62.80
20 2 48.46 30 0.69 62.81
30 2.25 49.9s 60 1.27 65.77
60 s.-oi 54-09
Data for boiling points in the svstem K2O -f CrOi.HiO determined by means
of the Beckmann apparatus, are also given.
The older data for KtCrOi and KsCrsO? are as follows:
Solubility of Each in Water.
(Alluard. 1864; Nordenskjold and Lindstrom, 1869; Etard, X894; Kiemecs. X854; TOden and SbeiK
■tone, 1884.)
Potassium Chrc
>mate.
Potassium Dichromate.
t-.
Gnuns
per xoo Grams Water.
Giamsper
xoo Gnuns WM»
0
58.2*
59 -St
60. 2t
s*
ss
10
60.0
61.2
62. s
7
7
30
61.7
63.2
64 -s
13
12
as
62. s
64.2
645
16
16
30
63-4
65.2
66. s
30
30
40
65.2
67.0
68.6
36
37
SO
66.8
69.0
70.6
34
37
60
68.6
71.0
72.7
43
47
70
70.4
73 0
74.8
S3
S8
80
72.1
75 0
76.9
61
70
90
73-9
77 0
79 0
70
83
100
75-6
79.0
82.2
80
97
"S
79 0
...
• • •
no
145
ISO
83.0
• . •
« • «
143
305
•Btoid.
$N.andL.
)A,K,T.udS.
529
POTASSIUM CHBOMATBS
SoLUBiLiTT OP Potassium Chromatbs in Water at 30**.
(Schreinemaker — Z. physik. Ch. 5& 83, '06.)
CompositioD in Wt. per cent of:
The Solution
The Residue.
-^ Solid
Phase.
eroentCrOs.
Per cent KsO.
FteoentGrOs.
Percent KflO.
0
±47
• • •
• • ■
KOH.9IUO
0.0
47.16
12.59
47-54
KiCrOt
0.1775
34.602
10.93
37-47
M
I -351
26.602
16.482
32.532
M
5-59^
20.584
37-131
39.922
M
15-407
19.225
27.966
29-377
M
«o.67
19.17
• • •
• • •
K,Cr04+ KaCwOy
19.096
17-30
37 64
22.61
KjCr^
"•35
7.88
• • •
• • •
«•
•
17-93
3-412
25-85
7.82
«4
43 SI
3.01
49-45
9.91
(1
44.46
3-245
53-94
12.40
KjCrjOr + KjCnOio
46.368
2.823
60.314
I2.9S5
KsCrgOio
49-357
2.353
63.044
11.684
K^Ti^ho+K^^
53-215
1.360
62.958
8.002
K^4Qis
62.55
0.796
67.944
6.731
t«
62.997
0.621
70.0
4.0
K«Cr4Qo + CiQi
62.28
Q.O
• • •
• • •
CrQi
100 gms. sat. solution in glycol, C?H4(OH)s.H20, cnntain 1.7 gms. K2Cr04at 15.4®.
100 gms. sat. solution in glycol, C2H4(OH)2.H|0, contain 6 gms. KsCr207 at 14.6®.
(de Coninck, 1905.)
100 gms. H2O dissolve 10. 1 gms. KjCrjOy at 15.5**. (Greenish and Smith, igox.)
100 gms. sat. solution in water contain 5.52 gms. KiCr207 at 4.81°, 15.17 K^^*
at 30.1 and 17.77 gms. at 35.33®. (Le Blanc and Schmandt, 29x1.)
100 cc. sat. aqueous solution contain 11.43 gms. KiCr207 at 20*^.
(Sherrill and Eaton, X907.)
Solubility of Potassium Chromate in Aqueous Solutions of Potassium
MOLYBDATE AT 25" AND ViCE VeRSA.
(Amadori, xgxaa.)
Gms. per xoo Gms. HfO.
Gms. per xoo Gms. HjO.
Gms. per xoo Gms. H|0.
K«Ci04.
K2MoO«.
K,Ci04.
K«MoO«.
X4CrO«.
K,Mo04.
64.62
0
14.13
98.72
4.92
165.4
49-59
15.37
10.07
118. 8
2.14
180.8
38.90
38-79 •
. 10.24
119. 9
1.70
183
33-21
50.96
7.12
6.37
137.8
157.2
0
184.6
Solubility of Potassium Chromate in Aqueous Solutions of
Potassium Sulfate at 25** and Vice Versa.
(Amadori, xgxaa.)
Gms. per xoo Gms. H^.
Gms. per 100 Gms. H/).
Gms. per xoo Gms. H/).
RiCeO«.
KjSO*.
K1C1O4.
K4SO4.
iKtCrOf.
KjSO*.
63.09
0.76
40.93
3.33
7.81
8.98
61.39
1. 17
27.36
4.82
4.36
10.25
58.40
1.84
20.83
5-72
1.94
10.86
51.81
2.36
14.65
7.12
0
12.10
100 cc. anhydrous hydrazine dissolve i gm. K2Cr04 at room temp. ) (Welsh and Brod-
100 cc. anhydrous hydrazine dissolve i gm. K2Crs07 at room temp. ) eison, xgxs.)
POTASSIUM CHB0MATE8 530
Freezing-point Data (Solubilities, see footnote, p. i) for Mixturbs of
Potassium Chromates and Other Compounds.
KtCrOi + KtCrsO;. (Groachu£F. 1908.)
KsCrO* + K1M0O4. (Amadori, 19x3.)
K,Cr,07 + KjMoiOt.
KsCr04 + KtS04. (Amadori, 19x5; GioKhuiT. 1908.)
K|Cr04 + K1WO4. (Amadori. X913.)
KjCrA + KjWiOz.
POTASSIUM CITRATE (CH,),C(OH)(COOK)t.H<0.
Solubility in Water.
(Avence resulU of Sddell, 19x0; Greenish and Smith, X901; KOhler, 1897.)
Gms. (CH|)|C(0H)(CXX>K)|.H^ per xoo Gms.
f. / * %
Sat. Soludoo. Water.
15 « 61.8 162
20 63.2 172
25 64.5 • 182 {d»= 1.518)
30 66 194
100 gms. HiO dissolve 198.3 gms. (CHi)iCOH(COOK)t + 303.9 gms. cane
sugar at 31.25**. (KOhler, X897.)
Solubility of Potassium Citrate in Aqueous Ethyl Alcohol at 25".
(Seidell, 19x0.)
When potassium citrate is added to aqueous alcohol of certain concentrations
the mixture separates into two liquid layers. A series of determinations made by
addine an excess of the salt to 10-15 cc* portions of several aq. alcohol mixtures
at 25 gave the following results.
«rf cr Mjt- Of Gms. (CHf)jC0H-
PH.^ <fc»of rwntf'in (C00K)^H^
in'^^t. Sat-lilution. sS.'ISSiSx. ^^
«-9 i;
ms.
t. Solution.
1.4920 o 60
ta ... ... 0.2
h 1.4930 o . 61.6
- \a ... 65.1 0.38
^ \h ... ... 62.5
7^-^ \h ... ... 62.3
81.4 0.8356 81.4 0.038
91.6 0.8139 91.6 0.016
99.9 0.7896 99.5 0.014
a = upper, alcohol rich layer, h = 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.
Wf CT Gms. (CH0,COH- «,, „ Gm8.(CH,),C0H-
cviX\i *fO« XCXX)K)tH5o pw^fr 4»of (COOK)jH,0.
hP^?t. SatsSution. Pergioobms. ,^^^^ Sat.^lution. P^JJ^^-
o 1.518 64
5 1.400 52
10 1. 310 45
20 I 177 31
30 1.085 21
5 40 1.005 12. \
5 SO 0-943 S-6
5 60 0.900 1.6
5 70 0.868 0.4
5 80 0.838 0.04
In one determination at 15®, made with alcohol of 59 Vol. per cent, 4.51 gms.
(CHt)iCOH(COOK)g.HtO were required to just cause clouding.
531
POTASSIUM CTANATE
POTASSIUM CTANATE KCNO.
Solubility in Alcoholic Mixtures.
(Erdnuum, 1893.)
Solvent.
80 per cent Alcohol + 20 per cent Water
80 per cent Alcohol + 20 per cent Methyl Alcohol
80 per cent Alcohol + 10 per cent Acetone
Cms. KCNO
per liter Solvent
at b.-pt.
62
76
82
POTASSIUM CYANIDE KCN.
100 ems. HtO dissolve 122.2 gms. KCN, or 100 gms. sat. solution contain 55
gms. kCN at 103.3*. (Griffiths.)
100 gms. abs. etnyl alcohol dissolve 0.87 gm. KCN at 19.5°.
100 gms. abs. methyl alcohol dissolve 4.91 gms. KCN at 19.5*. (de Bruyn, 1893.)
100 gms. glycerol dissolve 32 ems. KCN at I5<5°- (Ossendowski, 1907.)
100 gms. hydroxylamine dissolve 41 gms. KCN at 17.5**. (de Bmyn, 1892.)
F.-pt. data for KCN + KCl. KCN + NaCN, KCN + AgCN, KCN + Cui
(CN)t and for KCN -f Zn(CN)i are given by Truthe (1912).
POTASSIUM CHBOMOCYANIDE KiCr(CN)t.
100 gms. HiO dissolve 32.33 gms. KsCr(CN)« at 20*.
(Moissan, 1885; Christensca, 1885.)
POTASSIUM CHBOBCITHIOCYANATE K,Cr(SCN)«.4H,0.
100 gms. HsO dissolve 139 gms. salt. (Karsten, 1864-5.)
POTASSIUM CABBONYL RBBOCTANIDE KiFeCO(CN)t.3iHtO.
100 gms. HsO dissolve 148 gms. salt at 16°. (Moller, 1887.)
POTASSIUM FERRICTANIDE K«Fe(CN)6.
POTASSIUM FEBBOCTANIDE K«Fe(CN)6.3HtO.
Solubility of Each in Water.
(Wallace, 1855; Etard, 1894; Schiff, x86o; Michel and Krafift, 1858; Thonuen.)
Note. — The available determinations fall very irregularly when plotted on
cross-section paper, and the following figures, which are averages, are therefore
hardly more tnan rough approximations to the true amounts. The figures under
K4Fe(CN)« show the limits between which the correct values probably lie.
Gms. per xoo Gms. HfO.
Gms. per loo
> Gms. HA
» .
K,F*(CN)^
K,Fe(CN),.
0
31
13 ••
10
36
20 20
20
43
25 40
25
46
28 48
30
50
32 57
r.
K|Fe(CN),.
K«Fe(CN)^
40
60
38
70
60
66
52
83
80
• . •
66
89
00
...
76
91
104.4
82.6
100 gms. HtO dissolve 0.08946 gm. mols. = 32.97'gms. K4Fe(CN)6 at 25®, di^ of
sat. sol. = 1.0908. (Harkins and Pearce. 19x6.)
One liter of sat. solution in water contains 319.4 gms. K4Fe(CN)6.3HiO at 25°.
(Gnibe, 1914.)
Using the Harkins and Pearce figure for d^t this result corresponds to 34.3 gms.
K4Fe(CN)6 per 100 gms. HjO.
One liter of sat. solution in water contains 385.5 gms. KsFe(CN)6 at 23^.
(Gnibe, 19x6.)
POTASSIUM FERBICTANIDE 532
Onelitersat.sol.ino.4687nKOH;contain8»342.7gms.KjFe(CN)6at25®. (Grube, 1014.)
0.^28 " " 302.3 "
1.949 " " 215.1 "
100 cc. anhy. hydrazine dissolve 2 gms. KaFe(CN)6 at room temp.
(Welsh and BrodenoDt 1915.)
Solubility of Potassium Ferrocyanidb in Aq. Potassium Hydroxide
Solutions at 25^ (Grube, 1914.)
Gms. Gms.
Solvent. ^<:S2S*c?° P^ Solvent. ^^^^^^
per 1000 oc. x^nasc per looo oc.
Sat. Sol. Sat. Sol.
0.09984 nKOH 308.5 K4Fe(CN)«.3H,0 0.9415 nKOH 184.8 K4Fe(CN),.3BW)
0.2496 " 283.5 " 1-395 " 132. 1
0.4963 " 247.1 " 1.883 " 86.12
0.7036 " 217.4
Solubility of Mixtures 'of Potassium Ferrocyanide and Ferricyanidb
in Water and in Aq. Potassium Hydroxide Solutions at 25**. (Grube, 1914.)
Gms. per looo cc. Sat. Solution.
SoUd
Phase.
Solvent.
Water
0.4687 ft KOH
0.9628
1.949
KaFe(CN),.
338.1
309
275-3
200.8
Solid Phase.
K4Fe(CN)..
79 . 02 K,Fc(CN),+K4Fe(CN),.3Hrf)
66.64
55.19
35.95
it
II
i(
II
M
Solubility of Potassium Ferrocyanide in Aqueous Solutions of
Sodium Ferrocyanide at 25^ and Vice Versa. (Harkins and Pearce, 1916.)
Mob, per loop Gms. H«0. K^FeCCN).
Na4Fe(C:N)a. K^FeCCN),'.?" »«» Gms.
o 0.89459
0.05072 0.88272
0.06633 0.88544
0.12306 0.88088
0.25972 0.89II6
0.4900 0.91600
dy^ol Mols. per looo Gms. HaQ. Na4Fe(CN)f ^93}^
Sat. SoL BUFeCCN),. Na4Fe(CN),.Pcr"ooGm8. SatTsoL
0.87034 0.99000
0.91060 I. 01200
0.95879 I. 05177
1.0438 I.II59
329. 5
325.1
326
3244
328.3
337-4
364 -6
372.3
387.5
411
I. 09081 o 0.6818
1.0990 0.1327 0.7056
I. 10039 0.1789 0.7213
109350 0.2115 0.7253
I. 12796 0.2722 0.7610
1.17241 0.3532 0.7814
I . 19700 o . 5850 o . 8652
I.2II90 0.6III 0.8712
I . 22673 o . 6994 o . 8984
1.25789 1.0578 0.9588
205.25
214.47
219.23
220.44
231.29
237 -49
262.97
264.79
273 05
291 . 40
.0595
.0199
.0792
.1006
.1113
.1243
.1567
.1581
.1830
.2267
POTASSIUM ZINC CYANIDE K,Zn(CN)4.
100 cc. HiO dissolve 11 gms. KsZn(CN)4 at 20^
(Sharwood, 1903.)
POTASSIUM FLUORIDE KF.2H,0.
gms. HsO dissolve 92.^ gms. KF, or 100 gms. sat. solution contain 48 gms.
18**. Sp. Gr. of solution = 1.502. (Mylius and Funk, 1897.)
100
KFat
Solubility of Potassium Fluoride in Hydrofluoric Acid at 21*.
CDittc.
1896.)
rms. per xoo
Gms. HgO.
Gms. per too
Gms. H/).
Gms. per too
Gms.HK
HF.
KF.
' HF.
KF.
HF.
KF.
0.0
96-3
925
29.9
20.68
38 -4
1. 21
72.0
11.36
29.6
28.60
46.9
1. 61
61 0
12.50
30.5
41.98
61.8
3-73
40.4
13 -95
31-4
53-71
74.8
4 03
32.5
15.98
33-4
74.20
105.0
6.0s
30.4
17.69
35-62
119.20
169.5
533
POTASSIUM FLUORIDE
According to de Forcrand (i9ii)» a saturated solution of KF.2HsO in water at
18° has the composition i mol. KF -j- 3*90 mols. HjO = 45.3 ems. per 100 g^ms. sat.
solution. The solution in contact with KF.4HsO as solid phase, has the compo-
sition I mol. KF + 5.76 mols. HsO » 35.96 gms. KF per 100 gms. sat. solution.
Equilibrium in the System Potassium Fluoride, Ethyl Alcohol and
Water at 23**-26''.
(Frankforter and Fiary, 1913.)
The authors determined the binodal curve, the quadruple points and two tie lines.
Gms. per 100 Gms. Upper Layer.
Gms. per xoo Gms. Lower Layer.
r
■ \
KF.
CHiOH.
H,0.
KF.
CiHiOH.
H«0.
1.23
92.67
6.07*
45-33
0.67
54*
• • •
• ■ «
• 1
•
37.
82
1.70
60.49
1. 16
83.30
15
54
• 1
■
• • •
• • •
• • •
■ ■ •
• 1
( •
28
68
4.47
66.85
2.86
65.81
31
33
• i
1 •
• ■ •
• V •
4.47
57.4
38
13
20
90
II. 9
67. 2t
S-47
53 04
41
49
• • 1
• • •
...
* • •
V • •
•
k *
18
55
15.6
6s -85
6.93
47 52
45
55
■ <
1 •
• • •
• • •
8.84
41.28
49
.88
15
■7
21.8
63. St
9. 55
38.66
51
79
•
1 •
« • ■
• • ■
• • •
• • •
•
■ •
13
57
27.27
59.15
10.52
35.91
53
57
•
1 •
• • •
• • •
• ■ •
• ■ •
•
■ •
II
43
33.23
S4.34
xz
30
59
II
30
S9t
* Quad, points.
t Tie line.
1
\ Plait point approz.
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 23®-26*.
(Frankforter and Frary, 1913.)
Gms. per 100 Gms. Homogeneous Liquid.
Gms. per 100 Gms. Homogeneous Liquid.
KF.
CHjOH.
0.17
96.78
0.31
78.91
0.62
66.29
0.81
59-97
1.29
47.46
1.77
35.40
2.50
19-05
5.32
10.64
KF.
CsHtOH.
HiO.
8.IS
7.49
84.36
10
5
97
84.03
12.21
4
39
83-41
14.18
3
45
82.37
18.75
I
89
79-35
25-83
0
74
73.43
35.38
0
23
64.38^
47.62
0
039
52.34*
H|0.
3 -OS*
21.19
33-09
39 22
51.21
62.83
78.45
84.04
* Quad. pdnt.
One tie line was determined. In this case the upper layer contained 78.91%
CjHtOH and 0.31% KF, and the lower layer contamed 9.67% KF.
In this system, the effect of chang^e 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, 19x3.)
Binodal Curve for the System Potassium Fluoride, Isopropyl Alcohol
AND Water at 20**.
(Frankforter and Temple, 19x5.)
Results in terms of gms. per 100 gms. of solvent, alcohol + water.
Gms. per xoo Gms. Solvent.
Gms. per xoo Gms. Sohrent.
KF.
51.826
38.748
26.039
17. 8X2
CHiCHOHCHi.
1.555
2.965
6.525
12. 215
98.445
97.035
93.475
87 785
KF.
CHtCHOHCHt.
H^."
12.385
21.438
78.562
5.071
59 339
40.661
3.973
65 -455
34. 545
1. 70s
82.750
17.250
POTASSIUM FLUORIDE
534
BiNODAL CURVB FOR THE StSTBM POTASSIUM FLUORIDE, AlLYL AlCOHOL
AND Water at 20".
(Fiankforter and Temple, 19x5.)
The results are given in terms of grams per 100 gms. Alcohol + Water instead
of gms. per 100 gms. of the homogeneous mixture.
per 100 Gnu. Solvent.
Gms
. per zoo Gms. Solvent.
'KF.
CHt:CH.CH^H.
H^.^
KF.
CH«:CHCH^H.
HiO.
45-707
2.270
97 . 730
7.508
35.390
64.610
38.076
3-983
96.017
6.024
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
II. 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 Potassixtm Fluoride, Acetone, Water
AT 20".
(Fnmkforter and Cohoi, 1914.)
Gaa, per zoo Gms. Homogeneous Mixture.
Gms. per 100 Gms. Homogeneous Mixture.
KF.
46.3
44.24
33.34
29.86
25.74
20.28
16.31
12.40
(CHa)sCO.
trace
0.24
I
1.60
3.02
5.90
9.72
15.59
H|0.
53-7*
55.52
65.66
68.54
71.24
73.80
73.97
72.01
KF.
9.17
5
3.06
1.38
0.979
0.75
0.50
o
(CHi)tCO.
23.53
38.72
47.89
58.06
62.60
65.41
69.58
98
H^.
67.30
56.28
46.84
40.55
36.42
33.84
29.92
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 bmodal curves at temperatures between 0° 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, 19x6.)
Gms. per zoo Gms. Homogeneous Mixture.
Gms. per 100 Gms. Homogeneous Mixture.
' KF.
ch».co.CsH;.
HdO.
34.38
23.63
18.62
0.17
0.50
1.49
65.45
75.87
79.89
15.91
13.80
2.19
2.98
81.90
83.22
'kf.
CHf.CO.C|H».
H^.
10.50
4.87
84.63
5.70
9.93
84.37
3.96
12.42
83.61
0.84
21.23
77.93
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 (191 5).
Results for KF + KPO», KF + K4P1O; and KF + KaPO* are given by Amadori
(1912). Results for KF + KsS04 are given by Karandeef (1909). Results for
KF + NaF are given by Kumakow and Zemcznzny (1907).
535
POTASSIUM rOBBCATE
POTASSIUM rOBMATE HCOOH.
Solubility of Potassium Formate and of the Acid Salt in Water.
(Gioechttff, 1903.)
Solid Phase : HCOOK.
*
Solid Phase :
HCOOK.HCOOH.
t
Cms.
Mols.
Cms. HCOOK
Cms.
Gms.
Mols.
HCOOK
HCOOK
HCOOH
HCOOK
HCOOK
HCOOH
r.
per xoo
per 100
t**. per xoo
per 100
f.
per 100
S^L
Oms.
Mob.
GmB.
Gms.
Gmfl.
Sohition.
H*0.
Solution.
Solution.
Solution.
HCOOK.
— 20
72.8
57-4
0 60.4
39 0
0
36 -3
3-21
+ 18
76.8
71.0
25 69.8
4SI
19s
38 -2
2.96
so
80.7
89.8
SO 79-2
SI-2
39-3
40.8
2.6s
90
86.8
141 .0
80 90.7
S8.6
60
44.0
2-33
Z20
92.0
247.0
70
45-9
2.16
140
96.0
5"
90
S2.I
1.68
157
100. 0
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 QEBMANIUM FLUORIDE K,GeFe.
Solubility in Water.
(Winkler, 1887; Kruss and Nilson, 1887.)
100 gms. HjO dissolve 173.98 gms. KiGeFe at 18**, and 34.07 gms. at 100" (W.).
100 gms. HiO dissolve 184.61 gms. KsGeFt at i8% and 38.76 gms. at loo**
(K. and N.).
POTASSIUM H7DB0ZIDE KOH.
Solubility in Water.
(Pickering, 1893; at zs", FerchUnd, 1902;)
Gnu. KOH per
(Sms.
KOH per
f.
xoo
Cms.
Solution:
SdidPhaie.
f.
100 Gms.
Water. Solution.
SoHd Phase.
Water.
2.2
3.7
3-6
la
15
107
SI. 7
KOH.sH/)
20.7
22.5
18.4
<«
20
112
52.8
II
6s.2
44. 5
30-8
M
30
126
55-76
u
36.2
36.2
26. d
KOH.4HdO
325
135
5744
K0H.3H^+
32.7
77.94 43-8
ft
SO
140
58.33
KOH.H,0
zz
80
44-4
K0H.4Hs0+K0H.aHi0
100
178
64.03
KOH.H«0
23.2
8S
45-9
KOH.aHiO
125
213
68.06
II
0
97
49.2
II
143
3"-
7 75.73
M
10
103
50-7
M
•
Sp. Gr. of sat. solution at 15* - 1.5355-
100 gms. sat. solution in H|0 contain 50.48 gms. KOH at 15".
(de Forcrand, xQoQ.)
XOO gms. sat. solution in H«0 contain 53.1 gms. KOH at is"".
((Sreenish and Smith, 1901.)
POTASSIUM HYDROXIDE 536
Solubility of Potassium Hydroxide in Aqueous Solutions of Ethyl
Alcohol at 30". (deWaai, 1910.)
Cms. per 100 Gms. Sat. Sol. Gms. per xoo Gms. Sat. Sol.
, * , Solid Phase. , • v Solid Pbaae.
KOH. CtHiQH. H^. KOH. CAOH. H/).
55.75 O 44.25 KOH.2H4O 27.67 69.92 2.41 KOttaHtO
54.81 0.43 44.76 " 27.20 73.01 negative*
Two liquid layers are foimed here. 26 . 25 81 . 95
31 57.50 II SO KOttaHiO
28.99 65.07 5.94
* NegativeonaccountofreactionKOH+CAOH— »CsHi0K+H/).
Data for equilibrium in the system potassium hydroxide, phenol, water at 25^
are given by van Meurs (19 16).
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 lODATE KIO,.
Solubility in Water.
O^remen, zSsGa; at 30*, Meerbuzg, 1904.)
t**. o** 20** 30'' 40'' 60^ 80'' lOO*"
Cms. KIOi per 100 gms. HiO 4.73 8.13 11.73 12.8 18.5 24.8 32.2
TOO gms. HsO dissolve 1.3 gms. potassium hydrogen iodate, KH(IOs)i, at 15^
and 5.4 gms. at 17°. (Serullas.)
100 gms. HsO dissolve 4 gms. potassium dihydrogen iodate, KHt(IOt)s, at 15°.
(Meineke, 1891.)
Equh^ibrium in the System Potassium Iodate, Iodic Acid, Water at 30^.
Qleerbuxg, X905O
Gms. per xoo Gms.
Gms. per zoo
Gms.
Sat.
Sol.
Solid Phase.
Sat. Sol.
Solid Phase.
HIQfc.
KIQfc.
HIO,.
KIO,.
0
9. SI
^Qi
3-47
3. 59
KIQi.aHIQi (uast
0.65
9.49
" +KIQ1.HIQ1
4.80
2.90
II 1
0.65
8.90
KIQ1.IIIQ1
6.4s
1-35
II 1
0.67
6.6
u
9-3S
0.64
KIQ|.aHIQi
1. 14
457
u
12.04
0.44
II
1.69
3.63
11
17.50
0.30
M
2.02
3.10
u
31.20
0.52
M
3.34
2.10
II
53.64
0.68
If
5
1.32
II
62.52
0.72
tt
7.09
I
II
76.40
0.80
+hi(
8. 04
0.85
" +KI0i.aHI0i
76.7
0
HlOk
100 cc. anhydrous Hydrazine dissolve i gm. KIOs at room temp.
(Wdsh and Broderson, 19x5^
POTASSIUM PerlODATE KIO4.
100 gm«. HjO dissolve 0.66 gm. KIO4 at 13®, di^ of sat. solution = 1.0051.
(Bazker, z9oa.J
POTASSIUM IODIDE
Solubility in Water, Determined by the Freezing-point Method.
(Kremann and Kershbaum, X907.)
Gms. KI per goUd *. ^JS.riT' Solid
Sat. Sol. *^'**^ Sat.SoL ^^"^
— 12.5 38 Ice —22.5 52.1 KI
— 15 41.2 « —20 52.6 «
-17.5 44.6 " -15 S3. 5
-20 48 " -10 54.5 "
-22.5 51.2 « - 5 SS-4
-23.2Eutec. 51.9 «+Ki o 56.4 «
537
FOTASSIUM lODIDB
POTASSIUM IODIDE KI.
Solubility in Water.
(Mulder; de Coppet, 1883; Etard. 1894; Meustert 1905; see also Tilden and Shenstone, 1884;
Schreinemaken, 1892.)
Gms. KI per xoo Gms.
0
9
Water.
Solution
10
115. 1
S3 5
5
119. 8
S4.S
I
122.2
SS'O
0
"7S
56.0
10
136
S7-6
20
144
S9 0
2S
148
S9-7
30
IS2
60.3
40
160
61. s
SO
168
62.7
60
176
63 -7
70
184
64.8
80
90
100
no
120
S
7
9
II.
14
S
S
Gms. KI per 100 Gma.
Water. Solution.
192 65 .8
200 66.7
208 67.5
2IS 68.3
223 69. O
Ice Curve
25.7 22 s
42.6 29.9
s^'S 34.0
64.7 39-3
7S-S 43.7
Sp. Gr. of sat. solution at 1^.2° s 1.704. (Greenish and Smidi, igoxO
Individual determinations, in good agreement with the above resultSi are given
by van Dam and Donk (191 1), and by Greenish and Smith (1901).
S(X.UBiLiTY OF Potassium Iodide + Iodine in Water at 25*.
(Foote and Chalker. Z908.)
Gms. per too Gms. Sat. Sol.
KI.
29 ^S
28.91
26.84
27.18
27.14
I.
64.34
63.88
66.54
67.14
66.60
1-KL
34.89
34.97
39.70
39.96
39.46
Present in
Solid Phase.
Kland
KI.
KI,and
KIt
Gms. per xoo Gms. Sat. Sol.
KI.
25.88
35. S7
27.86
27.27
26.95
25.71
I.
68.79
(S9.OI
66.56
66.91
67.17
67.91
I-KI.
42.91
43.44
Present in
Solid Phase.
Klrand
Iodine
KI,
25.71 67.91 J '^
The experiments of Hamberger (1906) are discussed. (See also p. 326.)
Solubility of Mixtures of Potassiuic Iodide and Silver Iodide in
Water at o**, 30® and 50®.
(Van Dam and Donk, 191 z.)
Results at o^
Results at 30°.
Results at 50^
Gms. per xoc
> Gms. Sat. Sol.
KI.
Gms.perxoG
' A«I.
» Gms. Sat. Sol.
KI.
Gms. per xoo
Gms. Sat. Sol.
Solid Phase in
' AgL
A«I.
KI.
EochCaae.
0
56.1
0
60.3s
0
62.6
KI
9
S3
16
SS-5
10.7
S9.I
M
18
SI. 2
3S.8
46.9
22.8
SS'5
M
31.3
46.6
42.8
43.9
4S
43.2
M
37.9
44
44.1
43.2
S3-4
37-6
" +AgI.KI
37.6
42.7
47.7
40.9
S3.S
37.1
AgLKI
38
413
49.7
38.6
S3.S
36.6
" +AgI
28.1
36.4
42.8
38.8
53 S
36.5
Agl
26.6
34.6
29.4
37.6
39
38.1
if
6.S
26.1
10
31.4
28
36.7
u
IS
20.5
• • •
• • •
16
33.8
u
0.2
9.8
0.1
10.2
2.5
24.8
tt
27. s
48.7
• • •
• • •
• • «
« « •
AgI.aKT+KI
21
SO. 3
• • •
• « •
• • •
• ■ •
AgI.aKI
POTASSIUM IODIDE
538
Solubility of PoTASsiuiff Iodide in Dilute Aqueous Solutions of Ethyl
Alcohol at 25*.
(Aimstrong, Eyn, Hussey. and t^addiaoii, 1907.)
Wt. Per cent
d^Hin
Solvent.
O
Wt. Per cent
qOOHin
Solvent.
rf«oC Gm».KI
- It- , per 100 Cms.
Sat. Sol. 'sat. Sd. ^
1.7268 59.80 * 4.41
I. 14 I. 7154 59-41 X2.14
2.25 1.7042 58.95 18.73
100 gms. aqueous 94% ethyl alcohol dissolve 3.99 gms. KI at 17^.
100 ^ms. aqueous 08% methvl alcohol dissolve 1 7. i gms. KI at 1 7^
100 cc. of ethyl alcohol of chi "" 0.8292 dissolve 8.83 gms. KI at 15°, du of sat«
solution B 0.8989. (Gieenish and Smith, 1901^
rf«o£
Sat. Sol.
1.6833
1.6063
I . 5420
Gm8.KI
per zoo Gms.
Sat. SoL
58.08
54.93
52.08
(de Brujm, 189a.)
Solubility op Potassium Iodide in Absolute Alcohols.
(de Bruyn — Z. phyiik. Ch. lo^ 783, '9a; Rohland — Z. anocg. Ch. x8» 327, '98O
100 gms. methyl alcohol dissolve 16.5 gms. KI at 20.5°.
100 gms. ethyl alcohol dissolve 1.75 gms. KI at 20.5®.
100 gms. propyl alcohol dissolve 0.46 gm. KI at 15^-20® (R.).
Solubility
OP Pot
rASSIUM lO]
DiDB in:
Ethyl Alcohol
Aqueous Ethyl Alcohol at 18®.
(
of 0.9496 Sp. Gr.
Gms. KI per
Sp. Gr.
Weight
Gms. KI
Sp. Gr.
Weight
Gma.KI
t*.
100
of
per cent
per xooGms.
of
Alcohol.
per 100 Gna
Gms. Alcobol
Alcohol.
Alcohol.
^cohal.
Alcohol.
Alcohol.
8
67.4
0.9904
5-2
130-5
0.9390
45
66.4
13
69.2
0.9851
9.8
119. 4
0.9088
59
48.3
25
75-1
0.9726
23.0
TOO. I
0.8464
86
ZI.4
46
84.7
0.9665
29.0
89.9
0.8323
91
6.3
55
«7-5
0-9528
38 0
76.9
63
90.3
(Gersidiii
L — Aon. chim. phys. [4] S iss. ^3.^
Solubility of Potassium Iodide in Aqueous Solutions of Methyl Alcohol
AT 25**.
(Herz and Anders, 1907.)
Solvent.
Sat. Solution.
Solvent.
Sat. Solution.
J Wt. Per cent "
a*>.
Gms. Kl '
d^.
^t. Per cent
V
Gms.KI
H»'
CH^H.
per xoocc.
CHjOH.
per XOOCC
0.9971
0
I. 7213
102.9
0.8820
64
1. 185
40.33
0.9791
10.
.6
1.634
92.12
0.8489
78.1
1.066
28.05
0.9481
30
.8
1.460
71. 55
0.8167
93.9
0.9700
18.76
0.9180
47 ■
.1
1.325
55.6
0.7881
100
0.9018
13.28
Solubility
OF Potassium Iodide in Several Alcohols.
Alcohol
»
f.
Gms. KI per xoo
Gms. AlcohoL
f
Authority.
Methyl Alcohol
II. 4
13.5
(Timofeiew, 1894.)
u
u
12.2
14.6
u
u
13.5
16
w
it
ti
25
18.04
(Turner and Bissett, 19x3.)
Ethyl
tt
136
1.63
(Timofeiew, 1894.)
tt
it
25
^ 2.16
(Turner and Biaaett, 19x3.)
Propyl
It
12.2
0.731
(Thnofeiew, X894.)
<(
tc
25
0.43
(Turner and Biasett,
1913.)
Amyl
it
25
0.098
u
M
100 cc. sat. solution of K I in ethyl alcohol contain 1.585 gms. KI at 23^.
(Laune, 191 a^
539
POTASSIUM IODIDE
Solubility of Potassium Iodide in Liquid Methyl Alcohol at Tem-
peratures UP TO THE Critical Point.
(Tyrer, xgxo.)
(Determined by the Sealed Tube Method.)
Cms. Kl per
f.
zoo Gms.
CHgOH.
IS
14.50
30
16.20
50
18.9
80
22.5
ICO
25
f.
Gms. KI per
100 Gms.
CHgOH.
120
27.2
140
160
180
29.2
30.6
30.7
200
29.1
f.
Gms. KI per
100 Gms.
CH/)IL
220
27.5
240
24.8
245
22.6
247
21
250
13.8
252.5
7.6
Solubility of Potassium Iodide in Vapor of Methyl Alcohol Above
THE Critical Point.
(Tyrer, 1910a.)
Solvent,
Gms. CH^H
Gms. KI Dissolved
per xoo
Gms.
Solvent at:
a9o'.
per
I oc. Vapor.
asa'.
ayo*.
a8o».
O.I
0.3
• • ■
• ■ •
• • •
• • •
0.2
I
I
I
I
I
0.3
3.7
3.5
3.4
3.4
3.3
0.36
7.6
7.4
7-3
7.2
7
0.4
II. 8
"5
"3
II
• ■ •
0.45
18. 1
• • •
• • •
• • m
• • •
Data for the above system are also eiven by Centnerszwer (1910). This
author fives the crit. temp, as 266^ and the corresponding concentration as 8.64
gms. Kl per 100 gms. of the sat. solution.
Solubility of Potassium Iodide in Mixtures of Alcohols at 25**.
(Hers and Kuhn. 1908.)
In Methyl + Ethyl
Alcohol.
In Methyl + Propyl
Alcohol.
Percent
CHfOHin
Solvent.
O
4.37
10.4
41.02
80.69
84.77
91.25
100
Sat. Sol.
0.8015
0.8041
0.8071
0.829s
0.8794
0.879s
0.8908
0.9018
Gms. KI Per cent
per 100 cc. CJI7OH in
Sat. Sol. Solvent.
1.55
1. 91
2.2s
4.94
10.13
10.72
11.84
13 16
O
II. II
23.8
65.2
91.8
96.6
100
dmm of
Sat. Sol.
0.9018
0.8823
0.8629
0.8187
0.8045
0.8041
0.8041
Gms. KI
per zoocc.
Sat. Sol.
13.16
10.96
8.54
2.62
0.60
0.58
0.43
In Ethyl + Propyl
Alcohol.
Per cent
C>H,OHin
Solvent.
O
8.1
17.85
56.6
88.6
91.2
95-2
100
dy of
Sat. Sol.
0.8015
0.7983
0.7991
0.7988
0.8022
0.8027
0.8029
0.8041
Gms. KI
per xoocc.
Sat. SoL
1.55
1.46
1.37
0.75
0.52
0.49
0.44
0.43
Solubility of Potassium Iodide in Acetamide.
(Menschutlun, 1908.)
(Determinations by Synthetic Method.)
f.
Gms. KI per 100
Solid
f.
Gms. KI per zoo
Gms. Sat. Sol.
Phase.
Gms. Sat. Sd.
82 m. pt.
0
CHiCONH,
70
28.75
78
6.5
85
29.1
74
12.8
100
29.45
70
17.8
130
30.15
66
21.5
"
145
30.5
58
26.2
160
30.8
53 Eutec.
28.4
" +KI
175
31. 1
Solid
Phase
KI
If
M
tt
POTASSIUM IODIDE
540
Solubility of Potassium Iodide in Acetone and in Pyridine.
(von Lasscyittki, 1894; at 35", Krug and McElrqy, x893*)
Solvent.
Acetone
P)ni(iine
GmB. KI per xoo Cms. Solvent at:
.jc
308
xo'
aa'
0.26
2.38
«s*
S6' XI9'
2-93
1. 21
• • •
O.II
(Osaendowiki, 1907^
t 18.5".
100 gms. glycerol dissolve 40 gms. KI at 15.5^.
100 gms. 95% formic acid dissolve 38.2 gms. KI at 18.5^.
100 cc. anhydrous hydrazine dissolve 175 gms. KI at room temp.
(Welsh and Bxodenon, 19x5.)
100 gms. hydroxylamine dissolve no gms. KI at 17.5^. (de Bniyn, 1893.)
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
17- -i I--Lll^
f.
Sp. Gr. of
Solution.
Gms. KI
per xoo
f onnuui.
cc. Solution. Gms. Solution.
H^
0
1.6699
94.05
56.32
Hrf>
25
1-7254
102 . 70
59-54
CHiOH .
0
0.8964
II. 61
12.95
CHjOH
25
0.9003
13-5-14.3
14.97
GtHsOH
0
0.8085
1. 197
1.479
C2H5OH
25
0.7908
1.520
1.922
(CHrf)H),
0
1.3954
45.85
3103
(CHrf)H)t
25
I . 3888
47-23
33.01
CHjCN
0
0.8198
1.852
2.259
CHjCN
24
0.7938
1-57
2.003
CaHsCN
0
0.8005
0.34-0.41
0.0429
CJIsCN
25
0.7821
0.32-0.36
0.0404
CeHsCN
25
1.0076
0.051
0.0506
CH3NO,
0
I. 1627
0.314-0.366 0.315
CH,NO,
25
I . 1367
0.289-0.349 0.307
QHgNO,
25
■ • •
0.0019
• • •
(CH,)2C0
0
0.8227
1.732
2.105
(CH,)2C0
25
0.7968
1.038
1.302
C4H,0.C0H
0
• • •
15.10
• « •
C4H,0.C0H
25
I . 2014
5.62
4.94
CeHfiCOH
25
1.0446
0.343
0.328
C6H4.OH.COH
0
I.1501
1.257
1.093
C6H4.OH.COH
25
I . 1373
O.S49
0.483
C«H4.0CH,.C0H
0
I. 1223
1.520
1.355
C6H4.0CH,.COH
25
I.I180
0.720
0.644
CHjCOOCjHb
25
■ • •
0.0013
...
CH2CNCOOCH,
0
I.1521
3.256
2.827
CHjCNCOOCH,
25
I . 1358
2.459
2.165
CHiCNCOOCjHb
25
1.0628
0.989
0.930
541 POTASSIUM lODIDB
Solubility of Potassixtm Iodide at 20^ in Several Solvents Containing
Dissolved Iodine.
(OUvari, 1908.)
Gm. Mols. KI per Liter in Solvent Containing:
^^^^"^ 0.5 Gm. Mols. xTbm. Mols. 2.* Gm. Mob.
If per Liter. U per Liter. U per Liter.
Acetic Add 0.51X 1.460 2.080
Ethyl Acetate 0.490 1.400 x.980
Ethyl Alcohol 0.520 1.220 i-73o
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.) *
Gms. per 100 Gms. Upper Layer. Gms. per 100 Gms. Lower Layer. Solid
El SoT (CiHi)t0. 'kl 5o! {cSSSS. pJ»«-
... ... ... 59'^ 40.8 ... KI
O 3.9 96. Z 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. j)^ Gms. KI per 100 cc. Digt.
CANQfe Layer. B«0 Uyer. »*tio. CHaOH Layer. Aq. Uyer. R*t«>-
O.OOI14 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 + K1SO4 and KI + NaCl are p^iven bv Ruff and
Plato (1903). Results for KI + Agl are given by Sandonnini (1912a). Results
for KI -j- SOi are given by Walden and Centnerszwer (1903).
POTASSIUM lODOMXBCURATE (Thoulet Solution).
A sat. solution at 22.9°, prepared by adding KI and Hgli in excess to water,
contained 8.66% K, 22.^9% Hg, 52.58 (57.7) % I and 10.97 (".15)% HiO,
corresponding to 0.22 mot. alkali, o.ii mol. Hg and 0.45 mol. I. (Duboin, 1905.)
POTASSIUM MOLYBDATS KtMoO«
SC»LUBILITY OF POTASSIUM MOLTBDATB IN AqUBOUS SOLUTIONS OF POTASSIUM
Sulfate at 25® and Vice Versa.
(Amadori, 191 aa).
Gms. per xoo Gms. ^0.
Gms.
per xoo Gms. H/).
K«SO«. KaMoO«:
KiSOi.
KaMo04.
0 184.6
1.50
99-49
0.46 180.7
2.13
45-89
0.72 177
3.95
17.48
0.98 127.2
8.5s
4.73
1.27 107.5
12.10
0
Freezing-point data for KaMo04+ KiSO«, K,Mo04 + K1WO4 and KiMoiO
+ KsWsO are given by Amadori (1913).
POTASSIUM NITRATE KNOs.
Solubility Ice Curve and Supbrsolubility Ice Curve.
Gones, 1908.)
^ Gms. KN(^ per 100 Gms. Btf). Gms. KNQ^ per 100 Gms. H^.
ofCryst. Solubility Supersolubility ofCryst. Solubility SupenolubiUty'
Ice Curve. loe Curve. loe Curve. Ice Curve.
—I 3-336 I. Oil —3 ... 5.762
-2 7.582 3.538 -4 ... 8.694
— 2.8* 11.62 5.56 —5 ... II. 12
—5-3* ••• U.82
* Ciyoktydimte.
POTASSIUM MXTB4TE 54a
S(X.UBILITY IN WAIBB.
(Mulder; Andxae, 1884; Gcnidin, 1865: Etaid, 1894: Ort, 1878; at s'-as*. KOhler, 1897; Eider. 1904;
TDden and Shenatone, 1884; Berkeley, 1904.)
Average Curve.
^ Gma. KNO» per too Gma. ^ Gma.KNO» per 100 Gbm*
Water. Solution. Water. Solutioa.
o 133 II -7 70 13S S^o
10 20. 9 17.3 80 169 62.8
20 31-6 24.0 90 202 66.9
«5 37.3 27.2 100 246 71. 1
30 45-^ 31 -4 "o 30Q 75.0
40 63.9 39.0 120 394 79 -S
50 85.5 44.0 125 493 83.1
60 izo.o 52.0
-The very carefully determined figures of Berkeley are as follows:
^ dtoi Gma. KNOiper a. h^ Gma.KNO|per
Sat. Sol. xooGm8.IV>. '* Sat. SoL iooQms.Hfi'
0.40 1.081^7 13.43 60.05 1-3903 III. 18
14.90 I. 1389 25.78 76 1.4700 156.61
30.80 I. 2218 47.52 91-65 1-5394 210.20
44.75 1-3043 74-50 Ii4b.pt. 1.6269 311-64
1000 p[ms. HtO dissolve 384.48 gms. KNOt at 25°. (Armstroog and Eyze, X910-IX.)
One liter sat. solution in water contains 2.8 mols. = 283.11 gms. KNOs at 20^.
(Rosenheim and Weinheber, x9zo-zx.)
Recent determinations of the solubility of potassium nitrate in water, agreeing
satisfactorily with the above data, are given by Chugaev and Khlopin (19 14).
Solubility of Mixtures op Potassium Nitrate and Barium
Nitrate in Water.
(Euler — Z. physik. Ch. 4% 3x5, '04.)
t*. Sp. Gr. of Sat. SolutioB. Grama per too Grams HsO.
17 1. 120 13.26 KNOj+ 6.31 Ba(NOj),
21.5 ... 17.00 " + 7.58 "
30 1.191 24.04 " + 9.99 "
50 ... 49-34 " +18.09 "
Solubility op Potassium Nitrate in Aqueous Solutions op Nitric
Acid at o**.
(Encel — Compt. rend. 104* 9x3, '87.)
^. Gr. of Equivalents per xo cc. Solution. Grams per 100 cc. Solution.
Solutions, r ^ \ r *' \
1.079 12.5 KNOa o HNO, 12.65 KNO, 0.00 HNO,
9.9 " 5.87 " 10.02 " 3.71 "
1.093 ^-28 " 13.2 " 8.38 " 8.38 "
1. 117 7.4 " 21.55 " 7.49 " 13-58 "
1. 144 7-4 " 31-1 " 7-49 " 19-47 "
1.202 7.6 " 48.0 " 7.68 " 30.04 "
1.289 103 " 68.0 " 10.42 " 42.86 "
1. 498 28.3 " 120.5 " 28.64 " 75.95 *«
Freezing-point data for KNO» + HNOi are given by Dernby (1918).
543
POTASSIUM NITBATE
Solubility op Potassium Nitrate and op Acid Potassium Nitrates
IN Nitric Acid.
(Groschttff — Ber. 37, 1490. '04.)
Note. — Determinations made by the so-called thermometric
method, t.^., by observing the temperature of the disappearance of
the separated, finely divided solid from solutions of kno^m concen-
tration.
Gnuns per xoo Gms.
- 6
+ 14
17
19
32
21
21
20
- 4
-16.5
5
5
• per
Soiutiop.
24.4
32.6
34.8
37-2
445
47-8
48.6
SO -9
37-2
445
HNOa.
75-41
67.42
65.04
62.90
55-46
52.11
51.46
49 15
62.81
55 46
Solid
Phue.
KNOs.aHNOs (t)
(sUbU)
i«
M
It
ILNOs.jHNQi (I)
OabU)
«f
ti
KNOt.HNOs
(labil)
Gms. per xoo Gms.
22.5
23 5
25-5
27.0
29.0
30 -5
21.0
39 o
50
Sdiitipn.
47.2
47.8
48.6
49
50
50
49
50
51
4
I
9
4
9
7
HNOs.
52-93
52.11
51.46
50.78
49-94
49-15
50.78
49-15
48.32
Solid
KNOk.HNOs
** (stobO)
t(
KNQ1.HNO1
(labfl)
KNOs (UbU)
*• (aUbO)
C) Solution in HNOs-
(s) Solution in ILNOg.
Conduct op Acid Potassium Nitrate Towards Water.
Gms. per xoo Gms.
22
20.5
18
12
6
o
12
22
40
I. per
Soh]
ution.
HNQa.
445
55-
44.1
SS-
43-8
54-
43 0
53-
42 -3
52-
41.6
SI-
41 -3
SI-
40.9
SI-
39-9
49.
5
o
5
6
7
8
4
o
8
Solid
Phase.
KNQa.flHNOs
«i
•t
u
u
KNOs
50
61
63
60.5
56
43
17
-5
Gms. per xoo Gms.
• j)er
Solution.
387
36 0
34-5
30 -9
27. 6
20.8
7
5-54
II
HNOs.
48.3
44-8
43 -o
39-5
34-4
25-9
14.6
6.91
Solid
Phase.
KNOs
M
M
Solubility op Mixtures op Potassium Nitrate and Potassium
Chloride in Water,
(Btard -^ Ann. chim. phys. [7] 3, 283, '94: at ao^ Rador£f — Be(. 6^ 48af '73; Nicol -^ Phil. Mag. [5]
3x, 38s. '91)
i\
Gms. per loo Gms.
Solution.
XNOs. KCl/
Gms. per 100 Gms.
t*. Solution.
1LS0». KCl.
t\
Gms. per 100 Gms.
Solution.
KNOs. KQ.
0
5.0 20.0
30 16.0 21.2
70
39-5 17s
ZO
8.0 20.8
40 21.0 21.0
80
45-5 15-8
20
12.6 21.2
50 27.0 20.0
zoo
57-5 "-6
25
14.0 21.3
^ 33-5 19-0
Z20
69.0 7.7
FOTA88IUM NITRATl
544
Solubility op Potassium Nitratb in Aqueous Solutions op:
(Tourcn — Compt. lend, ijit 959, '00.)
Potassium Carbonate.
Potassium Bi Carbonate.
Scfults at mV*
Resnltsat
; X4.S*.
Obiob. pv Uter.
Gnii. per
Llt«r.
Mob. per Liter.
iLHCOs. KNO^
Grama pe
iCHCOs.
rlMet.
iiCOi.
KNOft.
W:o,.
]LNU».
KNO;.
0.0
8.228
0.0
225
0.0
2-33
0.0
236
048
1.85
66.4
188
0-39
2.17
39 -o
220
x.as
I 39
172.9
141
076
2.03
76.0
205
2SS
0.86
356-9
87
Z.16
1.92
116
194
3-94
0.64
544-9
65
J -55
1. 81
155
183
Result! at 9 j*.
Result! at af.
CO
32x7
0.0
326
0.0
3-28
0.0
332
0 59
8.62
81.6
265
0.89
2.84
89
287
J -35
1.97
186.7
199
1-33
2.65
133
268
9.10
1.46
290.5
148
1. 91
2-45
191
249
8.70
1. 14
373-6
"5
3 58
0.79
495-1
80
Solubility op Potassium Nitsatb in Aqubous Solutions op Potassium
Carbonatb at 24.2^.
(Kremaon and Zitek, 1909.)
jms-H^.
Solid
Phase.
KNOk
M
M
II
Gms. per
xoooGms.H/j.
Solid
KNOb.
376.8
285
161. 7
Z4I.8
K.(XV
0
130.3
348.4
371.9
KNQi.
73
38.8
3I-I
K.C0».
688.1
878.3
ZZI2.2
Phase.
KNOb
(1
" +K.COb
1000 gms.
HiO containing
I mol. KCl (]
[01. 1 1 gms.) dissolve 324.85
gms. KNOi
at 25'.
(Armstrong and Esne, z9zo-xz.)
Data for the system potassium nitrate, potassium sulfate, water at 35** are
given by Massink (1916, 1917).
Solubility op Mixtures op Potassium Nitratb and Potassium
Sulphate in Water.
(Ettler — Z. physik. Ch. 49b 3Z3t '04.)
Sp. Gr. of Sat. Solutioo. Grams per xoq Grams Water.
1.165
15
20
25
1. 210
24.12 KNO, 5.65X2804
30. 10 " 5.58
3612 " 5-58
a
Solubility op Mixtures op Potassium Nitrate and Sodium
Chloride in Water.
(Etard — Ann. cfaim. phys. [7] 3, aSj, '94; the older determinations of Rtidorff. Karsten, Mulder, stG«
scree well with those of Etard.)
Gms. per
Soiu
100 Gms.
Gms. per !
Solul
100 Gms.
Gms. per xoo Gms.
Solution.
*•.
tion.
%•.
tion.
••.
KNOs.
NaQ.
KNOs.
NaCl.
KNOl. NaQ.
0
13
24
40
30.5
19
Z20
73 8.0
xo
16
23
50
36
17
140
77 7-0
80
20
22
60
42.5
15
160
79.5 6.0
25
23
21.5
80
55
12
170
80.5 5-5
30
25
8O.5
100
67
95
545
POTASSIUM NITRATE
100 gmSk thPf simultaneously sat. with potassium nitrate and sodium chlo-
ride, contain 4I.I4 gms. KNOi + 38.53 gms. NaCl at 25"* and 168.8 gms. KNOi
+ 39-81 gms. NaCl at 80"*. (Soch. 1898^
Solubility of Potassium Nitrate in Aqueous Solutions op Sodium
Results at 20^.
Results at 30"*.
Sp. Gr.
Gms. per xoo Gms. H|0.
Solid
Sp. Gr.
Gms. per IOC
>Gms.H^.
Solid
Sat. Sol.
KNQ,.
NaCL
Phase.
Sat. SoL
KNQ,.
Naa '
Phase.
1. 167
31.49
0
KNOk
1. 261
46.48
9.82
KNOb
1.220
33 41
9.94
If
1.302
47.08
20.18
M
1.267
34.93
19.44
M
1-343
47.24
29.86
II
1.3"
36.41
29.46
<4
1-372
49.24
38.72
** +Naa
1.344
37.30
37.73
" +Naa
1.342
38.36
38.55
NaQ
1-330
31.41
37.57
Naa
1.298
25.32
38.23
II
1.283
19.56
37.51
li
1.258
12.15
37.38
M
1.243
9.76
36.73
ft
1.202
• • •
36.30
M
Results at 40^.
Results at 9I^
1.288
64.74
0
KNOb
1.552
202.8
0
KNOb
1.320
64.66
11.32
If
1.573
204.2
12.81
II
• • •
64.05
23.41
If
1. 601
208.1
28.45
u
1.396
64.13
35.08
M
1.645
213.3
37.92
II
1. 411
64.77
38.79
" +Naa
1.660
218.8
39.08
" +Naa
1-376
52.81
39.51
Naa
1.607
175.8
40.87
Naa
1.323
34.98
38.98
11
I-517
126.9
44.33
II
1.267
17.33
37.74
II
1.378
57-53
42.90
M
At the higher temperatures, results for NaNOs in certain solutions are reported.
Solubility of Potassium Nitrate in Aqueous
Nitrate and Vice Versa. (Leather and
Sp. Gr.
Sat. Sol.
I.317
1.403
1.472
1.544
1.520
I.481
I.451
1.406
Results at 30"*.
Gms per xoo Gms.
KNOi.
45.73
47-25
50-93
54.34
47.67
30-25
14.30
O
NaNOk.
25-90
52.53
79.27
103.3
103. 1
I0I.6
99.10
95.90
Sp. Gr.
Sat Sol.
Results at 40^.
Gms. per xoo Gms.
52^
1.358
1.428
1.505
1.570
1.573
1.526
1.476
1.42 1
KNOk. NaNOt.
63.21 23.85
Sp. Gr.
Sat. Sol.
Solutions of Sodium
Mukecji, X9X3.)
Results at 91 ^
Gms. per xoo Gms. Solid Phase
Hfi.
63.86
66.44
74.06
68.72
43.92
49.79
79.46
I16.2
116.7
II2.2
20.33 109.9
o 105.2
615
674
751
790
774
695
610
521
NaNOk.
43.4 KNOb
92.90
156.2
KNOk.
200.8
207.2
229.5
251.8
211. 7
128.5
55.75 I73-I
o 160.8
m
Each Que.
II
II
206.5
200
186
" +NaN0b
NaNOk
II
If
11
Results at 20* are also given.
Solubility of Potassium Nitrate in Aqueous Solutions of Sodium
Nitrate and vice versa at 20°.
(Camelly and Thomsoa — J. Oi. Soc. 53* 78a, '88; Nicol — Phil. Mag. 31* 369, V-)
KNO, in Aq. NaNO, Solutions. NaNO, in Aq. KNO, Solutions.
Grams per xoo
Grains HflO.
Grams per xoo Grams HgO.
NaNOs.
KNOs
KNQ|.
NaNOi. '
0
31.6
0
88
10
30.5
10
90
30
31 0
30
9a
40
33 0
as
93
60
35 S
30
94
80
41 0
35
96
POTASSIUM NITRATE
546
SOLUBIUTY OF. POTASSIUM NiTRATB IN AqUBOUS SOLUTIONS OF SODIUM
Nitrate and Vice Versa at 10^ and at 24.2^.
(Kremann and Zitek, 1909.)
f.
xo
10
10
24.2
24.2
Gms. per looo Gnu. Hfi.
KNO>.
208.9
301.9
O
377-3
$90
NaNQi.
o
848.3
80s
o
346.7
Solid Phase. t*.
KNOb 24.2
" +NaNOb 24.2
NaNOk 24.2
KNOi 24.2
u
Gms. per xooo Gms. H^.
KNO|.
422
437
123.6
O
NaNOi.
931.3
1019
910.6
913
Solid Phase.
KNOb
+NaNOb
NaNOb
u
•I
Solubility of Potassium Nitrate in Aqueous Solutions of Silver Nitrate
Gms. per xoo Gms. Sat. Sol.
AT 30" AND Vice Versa.
(Schxeinemakers, z9o8^-o9.)
Gms. per loo Gms.Sat. SoL
KN0|.
31-3
30.4s
29.22
26.58
25.02
AgNQ,.
O
II. 51
23. 59
3909
46.38
Solid Phase.
KNOb
tt
u
u
u
+AsN0b.KN0b
KNQ,.
17.38
13.44
XX. 22
5.53
O
AgNO,.
57.85
65.08
69.01
71.65
73
Solid Phasft
AgNObJLNOb
M
11
+AgN0b
AgSCh
M
Solubility op Mixtures of Potassium Nitrate and Silver Nitrate
f.
o
xo
20
25
Gms. per xoo Gms. Sol.
IN Water.
(Etard. 1894.)
Gms. per xoo Gms. Sol.
KNO,.
13.5
19
23
25
AgNQi.
43
44.7
47
48
30
40
50
60
KNOk.
26.8
29.6
32
33-5
AgNO,.
49 4
51.5
54
54.8
80
100
120
140
Gms. per xoo Gms. Sol.
KNO,.
36.2
38.3
40
41.5
AffNOb.
551
55.3
55.6
55.8
Solubility of Mixed Crystals of Potassium Nitrate and
Nitrate in Water at 25**.
(Herz, 1905; Fock, 1897.)
Gms.
per Liter.
Mg. Mols.
per Liter.
Mol. Per cent
AgNO^
KNO^.
AgNQ,.
KNQ»
AgNObin
Solution.
45 9
321.8
270
3180
783
no. 7
322.6
651.3
3184
16.96
176.8
333.7
1040
3298
23.97
259.6
364
1528
3597
29.81
365.6
456.4
2151
45"
32.28
507.9
387.2
2988
3816
43-85
745.9
398.6
4388
3960
52.70
Silver
Mol. Per cent
AgNaih
SoSlPhaafe.
0.2896
0.6006
0.9040
1.054
1.604
2.439
8.294
Solubility of Potassium Nitrate in Aqueous Solutions of Strontium
Nitrate and Vice Versa at 20" and at 40*.
(Findlay, Morgan and Morris, 19x4.)
Gms. ner 100 Gms.
Sat. Sol.
KNQ,. Sr(N0i),.
Gms. per
zoo Gms.
f.
Solid Phase.
f.
Sat
.Sol.
Solid Phase.
KNQ,.
Sr(N0i)t.
20
22.90 5.49
KNOb
20
12.65
41.12
Sr(N0b),.4H|0
20
21.70 9.17
20
10
40.70
<i
20
21.01 17.10
40
30.26
23.70
KNOb
20
19.60 31.24
40
26.90
38.52
« +Sr(N0b),.4DW>
20
19.49 34.91
40
22.50
40.22
Sr(N0b)i.4fiV)
20
19.69 39.56
" ^-Sr<NOi)^4HiO
40
II. 19
44.19
tt
20
17.56 40.37
Sr(N0k),.4H«0
40
0
47.7
u
1000 gms. H|0, simultaneously saturated with both salts, contain 552 gms.
KNO$ + 1074 gms, Sr(NOj)j at 25**, (LcBlanc and Nayts, 1890.)
547
POTASSIUM NITRATB
Solubility
OP Mixed Crystals op Potassium Nitratb and Thal-
lium Nitrate in Water at a
'5^
(Fock.)
Grains per liter.
TINO3. KNO,:
Mg.Mols.
> per Liter.
Mol. ner cent Sp. Gr. Mo
TINO3 of
in Solution. Solutions, in S
iLper cent
TINOt
TlNOi.
KNOa.
oUdPhaK.
COO
351-0
0.0
3468 . 2
0.00
1.2632
0.00
2.37
329.0
8.9
3251-5
0.43
I. 1903
0.08
6.15
332.4
^3^^
3285.1
0.70
I. 1956
0.20
17.64
333-7
66.3
3298.1
1.97
1.2050
0.57
49-74
333-3
186.9
3294 -4
5-37
1. 2196
1.78
63.60
321.0
239.0
3172.4
7.01
1.2436
2.19
86.18
330-5
323-8
3265.8
9.02
I. 2617
2.77
"3-8
428.3
465.2
4232.6
9.90
1.2950 1
6.00
27.04
1013
245-1
380.6
2423 -3
13-58
1.2050 (
nzz
116. 1
0.0
463,1
0.0
100.00
1.0964 100.00
Solubility
OP Potassium Nitrate in
Aqueous Alcohol Solutions.
(Gerardin — Ann. chim. phys. [4] s z5Xt '<$5')
Grams KN0» per
xoo Grams Aqueous Alcohol of Sp. Gr.:
f.
0.9904
0.984J
0.9793
0.973^
-09571
0.939 0.8967
0.8429
Wtf^o.
wt^-e
-X3^
Wt.%.
■■19.x
Wt.%.
»30 —40 —60
Wt.%. Wt.%. Wt.%
—90
Wt.%.
lO
17
13
10
7
4.5
3 I
0.2
i8
22.5
18.5
145
10
6.2
4-5 1-6
0.3
20
24
20
16
II
7.0
5 2
0.3
25
29
245
20
13-5
9.0
6.5 2.5
0.4
30
36
30
25
17
"•5
8 3.0
05
40
52
43
36
27
16.5
11 4
0.6
50
72
61
50
38
23.0
16 6
0.7
60
93
79
69
52
31.0
21 8
I.I
Solubility op Potassium Nitrate in Aqueous Alcohol at i8**
(Bodl&nder — Z. physik. Ch. 7, 3x6, V*)
£l<
I
I
I
I
I
I
I
I
Gr.of
ution.
1480
1085
lOIO
0805
0755
0655
0490
037s
Gms. per xoo cc. Solution.
CsHtfOH.
3
5
8
9
14
16
19
30
24
69
06
08
27
97
HaO.
89.80
87.44
86.26
83.18
83.10
77-93
76.36
72.93
KNOs.
25.0
20.11
18.60
16.18
15-39
14.54
12.27
10.8
Gr.cf
ution.
I. 01 20
0.993s
0.9585
0.9450
0.9050
0.8722
0.8375
Gms. per xoo cc. Solution.
CsH^H.
23 -33
28.11
37-53
42.98
51-23
61.65
69.60
HsO.
69.81
64.74
54.21
48.15
27.32
24.74
13-95
KNOi.
8.06
6.50
4. II
3-37
1-95
0.83
0.20
Solubility op Potassium Nitrate in Dilute Ethyl Alcohol at 25*
(Armstrong and Eyie, z9xo-xx.)
Wt.%
C^OHin
Solvent.
O
1. 14
2.25
4.41
Gms. KNOb
Der xoo Gms.
Sat. Solution.
27.77
26.69
25.79
23.81
POTASSIUM NITRATE
548
Solubility of Potassium Nitratb in Aqubous Alcohol and in Aqueous
Acetone.
(Batukk, 1896.)
In Aqueous Alcohol.
In Aqueous Acetone at 40*.
Wt Per cent
Akohol.
0
Cms. KNOk per 100 Gms. Aq. Akoliol.
At 3o'. At 40*.
45.6 64.5
Wt. Per cent
Acetone.
0
Gms.KNOb
per 100 Gms.
Solvent.
64.5
8.25
17
32.3
22.4
47.1
33-3
8.5
16.8
51-3
38.9
25.7
35
15. 1
11.4(34.4*0
24.1
16.7
25.2
34.3
22.8
24.7
44.9
7
11.6 (44*)
44.x
17
54.3
65
75.6
88
4-5
2.7
13
0.4
7.2(55^
4.4
0.6 (88. si
53.9
64.8
76
87.6
II. 9
7.2
3
0.7
100 gms. HfO saturated with sugar and KNOt dissolve 224.7 gms. sugar +
41.9 gms. KNOs, or 100 gms. of the saturated solution contain 61.36 gms. sugar
+11.45 gms. KNOi at 31.25^ (KOhkr, t897<)
S(H«UBILITY OF POTASSIUM NiTRATB IN AqUEOUS SOLUTIONS OF MSTHYL
Alcohol, Ethyl Alcohol and Mixtures of the Two at 30".
(Srhrrinrmakers, 1908-09.)
In Aq. CHiOH.
In Aq. C,H,OH.
InAq.(CHiOH4
CiHiOJ
Gms. per 100 Gms. Sat. SoL
Gms. per xoo Gms. Sat. Sol.
CtHftOH. KNOk.
Gms. per 100 Gms. Sat. Sol.
CHiOH. KNQ^
(CHiOH+CiH^H)
KNOb.
0 31.3
lO.I 20.7
0
31.3
7.8 23.3
23.8 12. I
12.7
18.9
173 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 S'S
47.8
5.1
57 3.8
76.8 0.88
56.4
3.5
98.58 0.43
92.3 015
74.8
1.2
* The mixture contained 5z.7% CH/)H and 48.3% CAOH.
100 gms. trichlorethylene dissolve o.oi gm. KNOi at 15^ (Wester and Brains, 1914-)
100 cc. anhydrous hydrazine dissolve 14 gms. KNOi at room temp.
(Welsh and BroderMn, 1915.)
100 gms. aq. 40 weight % CsHtOH, simultaneously saturated with the two
salts, dissolve 13.74 gms. KNOs + 15.78 gms. NaCl at 25^. (Soch, 1898.)
Simultaneous Solubility of Potassium Nitrate and Silver Nitrate in
Aqueous 51.6 Per cent CsH»OH at 30®.
(Schretnemakers, 1908-09.)
Gms. per 100 Qna. Sat. Solution.
KNO^ ' AgNOi.
4.8 O
4.55 5.15
4. II 16.47
4.26 21.28
2.62 36.94
o 37
Solid Phase.
KNOb
'* +AgN0b.KN0b
AgN0b.KN0t+AgN0b
AgNOb
Fusion-point data (solubilities, see footnote, p. i), are given for KNOi + KNOi
by Menegnini (1912); for KNOs + AgNOi by Usso (1904); for KNOi + NaNOi
by Carveth (1898) and by Hissink (1900); for KNOi + Sr(NOi)i and KNOj
+ NaNO, + Sr(NOi)i by Harkins and Clark (1915); for KNOi + TlNQi by
Van Eyk (1899, 1905).
549 POTASSIUM NITBITS
POTASSIUM NITRITE KNOs.
Solubility in
Water.
(Oswald, 1912,
«9«4.)
Gms. KNO^
SAlirl
Gnu-KNOb
f.
per xooGms.
Sat. Sol.
ovuu
Phase.
«*.
per too Gms
Skt.SoL
- 4.1
16. 1
Ice
+ 175
74-5*
- 7.6
24.1
«
25
75-75
-13.8
40.2
M
40
77
-18.6
SO. I
<«
55
77-5
— 24.6
61.7
M
75
78-5
-30
69.8
M
100
80.5
—31.6 Eutec.
71.8
"+KNOb
III
80.7
- 6.S
73-2
KNOk
119
81.15
0
73-6
fi
"5 .
81.8
SoHd
Phase.
KNOi
• dvA ■■ 1. 6464-
100 gms. HsO dissolve about 300 gms. KNOs at 15.5^ ^ (Diven, 1899.)
The figure 138.5 gms. KNOs per 100 gms. HsO at 15°, given by von Niemen-
towski and von Roszkowski (1897), is evidently low.
Solubility of Mixtures of Potassium Nitrite and of Silver Nitrite in
Water.
(Oswald, X9I4')
Results at 13.5*. Results at 25**.
Gms. per 100 Gna. H/). Gms. per iqo (jins. H^.
£n5! AgNQi. KN0». " AgNQi.
Solid Phase in Each Case.
18 2.36 23.1 5.3 AgN0b+K,A&(NQi)4.H,0
276 26.3 279 39.3 KN0i+K,A&(NQi)4.H,0
Of the two layers obtained by mixing an equal volume or more of 96% ethyl
alcohol with a nearly saturate aqueous solution of KNOs, the lower contains
71.9% KNOs and the upper, alcoholic, 6.9%. With methyl alcohol there is no
separation into two layers. (Donath, x9xx.)
POTASSIUM OXALATE KsCs04.4HsO.
Solubility of Mixtures of Potassium Oxalate and Oxalic Acid in
Water at 25°.
(Foote and Andrew, 1905.)
Gms. per xoo Gms. Solution. Mols. per 100 Mols. HsO.
HtC04.
K.QO4.
10.2
• • •
10.31
0.04
9.26
013
3-39
0.63
2.06
4.26
1. 16
11.50
0.99
16.93
0.8s
21.08
0.82
21.49
0.64
23 52
0.57 .
24.88
0.43
27.52
• • •
27.40
H.CO4.
KtCO*.
2.274
• • •
2.302
0.005
2.046
0.016
0.707
0.071
0.440
0.49s
0.266
1.427
0.240
2.235
0.221
2.928
0.211
2.998
0.169
3 361
OIS3
3.617
0.122
4.14
• * *
4.09
1
1
SoUd Phase.
H|C^4-2H^
H,Crf)4.2H/)+H,K(CO«)f.aHiO
Double salt H«K((V>4)i.aHflO
H«K((^4)-3lI/)+HKC.04
Double salt BKCfi^
HXCA+HsE4((^4)t.aH^
Double salt HtE4(C|0Js.sH^
BiK4(C|04)i sH^+K«Ca04.H^
K,C,04.H,0
POTASSIUM 0XALATI8
550
Equilibrium in thb System Potassium Oxalate, Oxalic Acid, Water at
O**, 30® AND 60**.
(Koppel and Cahn, 1908.)
Results at o"*.
Results at 30^
Results at 60*.
Gms-Der
xooGms.
Gins.per
xoo Gm>.
Gixtt.per
xooGms.
Sol.
Sd.
^
.Sol.
Solid Phue in EKfa Case.
CA.
' IW).'
QQi.
K*0.
CA.
K*0.
2.72
• • •
9-97
• • *
24.75
• • •
H^QO«.iHdO
2.91
0.226*
10. IS
O.IO
« • •
• • •
u
2.98s
0.342*
■ • •
• • •
■ • •
■ a •
M
2.827
O.I2S
10.23
0.34
25.70
0.46
- +KH.(QOJt.aW)
2.34s
0.145
• • •
■ • «
• • •
• « •
M M
1. 471
0.195
7.28
0.33
25.80
0.54
KH«(QO«)».aH^
0.823
0.240
4
0.41
22.06
0.58
u
0.799
0.454
3.08
o.so
20.17
0.67
M
1. 173
0.78s
2.38
1.002
14.25
0.90
M
1. 381
0.962
2.98
1.79
9.82
1.48
M
I.S4S
i.iSS
« • ■
• • •
6.95
2.244
M
1.666
1.273
4.24
2.76
9.17
S.6O
" +KHCA
I.7S4
1.479
4.26
3.38
8.81
6.37
KHC^4
2.627
2.858
5. 44
5.43
10.17
10
u
3.772
4.422
6.66
7.27
12.36
13.40
M
4.292
5.161
8.64
10. OS
14.10
16
II
4. 975
6.088
10.03
12.01
15.35
17.80
U
5.652
7
10.80
12.94
16.07
18.89
" +(K.Q04)ACA.2H^
6.27
7.87
11.47
14.13
16.51
19.59
(K,C|Q4),.H«Q0«.aH^
7.63
9.7^
12.16
15."
16.80
20.10
<(
8.66
II. Z4
12.32
15.37
16.95
20.34
II
9055
II. 5B
12.90
16.23
17.14
20.70
" +k:«Q04.h^
8.826
11.52
12.36
16.14
16.71
20.41
km:>4W>
5.215
12.33
8.52
15.03
15.94
20.11
u
2.23
14.80
4.53
IS- 55
15.06
19.66
M
1.24s
16.82
1.87
18.17
8.82
19.25
M
0.871
18.4
0.74
22.32
2.04
23.09
It
o.sii
20.91
• • •
• • •
0.434 29
M
0.325
23.30
« • •
• • •
0.365
31.40
II
0
41-31
0
46.79
0
51.34
KOH.TV)
* Supenatunited.
t About.
Equilibrium in the System Potassixtm Oxalate, Oxalic Acid, Water
AT 25*.
Gms. per
Sat.
xooGms.
\ii»iii^, .a^mt^Aua
100 Gms.
Sol.
Sdid Phase.
Sol. Solid Phue.
CA.
' CA.
K<0.
8.29
0 H|CsO«.aII/)
3.079
2.052 KH,(C04),.3H^
8.278
0.045
•'+KH,(C04),.aIV)
3.450
2.360 " +KHCA
7.412
0.064
KB,(Q04),.2H^
3-793
3.199 KHQO4
2.827
0.238
II
5.457
5.919 "
•2.007
0.346
M
9.816
1 1 . 96 « +aK.C,04.HiCi04. jH/>
1.734
0.567
U
12.365
15.71 aK.Q04.H.Ci04.2H/)+K«CA«)
2.67s
I. 714
•1
11.85
15.51 K,Q04.H/1
Similar data at 15^ for the above system are given by TunKfleisch and Landrieu
(1914a).
551 POTASSIUM OXALATES
SOLUBILITIBS IN THE StSTBM POTASSIUM OXALATE, OXALIC AciD, WATER AT
THE CRYOHYDHig POINTS.
(Koppd and Cahn, 1908.)
(Temp, of Equilibrium of Solution with Ice.)
fofloe Qaa,perioo « i-j uu ' t* of Ice Gma. dct xoo e^« j tm..,^
\^ Gms. ^. Sol. Solid IW •scpaiS: Gms. g. SoL ^oUd Ptoe,
-.0.95 2.64Z ... H9C|04.sH^ — 4.45 6.902 8.820 (E«Cy04)|.H|Q04.2H^
—0.90 3.720 0.0466 '* +KHt(C/)^»2^0 — 5.20 7.616 9.74
—0.52 1.672 0.0602 KBtCCiOJfaH/) — 5.32 7.696 9.84
—0.25 0.643 0.210 " — 5.97 8.51 XI. 01 *• +KtC/)4.HflO
—0.58 1.229 0.823 " — 6.5s 6.742 I0.4S K«C^4.B^
—0.78 1.648 1.234 " +KHCA — 8.10 4.999 10.86 "
— 1.50 2.707 2.950 KHC1O4 —10.30 3.358 11.76 ••
— 2.10 3.687 4.363 " —13.60 1.854 13.08 •*
— 2.78 4.576 5.50 " —1740 I.200 14.55 **
—3.4s S.681 7.05 " +(S:tC|04;s. —23.80 0.606 16.89 "
H|Q04-aH^
SOLUBILmES IN THE SYSTEM POTASSIUM OXALATE, OXALIC AciD, WaTBR AT
THE Boiling Points.
(Koppd and Cahn, 1908.)
Gms. per
100 Gms.
Gms. per
CA
TOO Gms.
t*ol
B.pt.
sS.
Sol.
Solid Phase.
t*of
B.pt.
Sol.
Solid Phaae.
CA.
KflO.
105.S
39.84
5.25
KH,(Cj04)t.aH,0
102.8
19.10
18.25
KHC64
X04.9
36.95
5.83
u
103.25
21.11
21.71
$t
104.3
32.75
5.97
u
107.7
25.19
27.91
" +K.CO4.H/)
103^
27.64
9.12
u
106.35
22.04
26.45
K.Crf)4.H,0
102.9
27.46
"43
"+KHC,04
106.25
19.17
25.02
i<
102.5
23.36
10.50
KHCrf)4
108.25
12.73
27.69
(1
X02.4
x8.8i
X2.29
<i
III.8
535
30.40
M
From the [)receding tables the following results for the solubilities of the
pure oxalates in water are obtained.
Solubility op Potassium Oxalate, KtCi04.HiO in Water.
«•. :
Lims. per zoo Gms
. Sat. Sol.
Solid
Phase.
f . s
ms. per zoo Gms. Sat. So
CA + KiO -K,C04.
t. Solid
CA + K/)-
■K,C^4.
■" Phase.
— 0.78
1.31 1.71
3.02
Ice
30
12.36 16.14 28.50
KA04.HiO
- 1.49
2.48 3.20
5.68
u
40
X3.20 17.22 30.44
14
— 2.50
3-99 5.20
9.195
u
so
14.14 1846 32.60
tt
— 3.22
5.15 6.705
"•855
(f
60
15.06 19.66 34.72
u
- 5.88
8.429 1 1. 01
19.43
" +K,C04.H,0
70
15.94 20.81 36.75
M
0
8.83 11.52
20.35
K«C,04.HiO
80
16.86 22.02 38.875
U
+10
10.48 13.69
24.17
it
90.2
17.73 23.14 40.90
<l
20
11.57 15."
26.675
u
xo6.2*
19.17 25.02 44.19
tt
•b.pt.
100 gms. sat. aq. sol. contain 20.62 gms. K1C1O4 at o^ d « 1.161. (Engel, z888.)
The results o£ Hartley, Drugman, Vlieland and Bourdillon (1913) and of
Colani (19 16), for the solubility of neutral potassium oxalate in water, agree
satisfactorily with the above.
Solubility of Potassium Bioxalatb, KHC1O4, in Water.
(Koppel and Cahn, Z908.)
rGms. per zoo Gms. Sat. SoL _ ,. . «.
< * » Solid Phase.
60 8.75 6.50 KHC/)4
x02.4b.pt. x8.8i X2.29 '*
The KHC1O4 is decomposed to the less soluble tetroxalate- at temperatures
below 50*.
POTASSIUM OXALATES
552
Solubility of Potassium Tbtroxalatb, KHtCCiOOs.aHiO, in Water.
(Koppel and Cahn, 1908.)
f.
— o. 25 cryohydrate
o
30
60
103.sb.pt.
Cms. KHtiCfi^
100 Gnu. Hfi.
0.99
1.27
4.30
"•95
72.17
Solid Phaae.
u
Solubility of Mixtures of Potassium Oxalate and Other Salts in
Water. (Cobni. 19x6.)
Results at I5^
Gms. per xoo Gms. Sat. SoL
Results at 50^
Gms. per xoo Gms. Sat. Sol.
10.03 KtCK>4+ 19.19 KCl
23.SS " + i.82K,SOi
20.39 " +11.60 KNft(i9*')
Solid Pbaae in
k Each Case.
15.18 KjCi04+ 20.26 KCl K^co«.H^+Ka
31.06 " + 1.99K1SO4 " +Ki3Q,
19.63 " +28.29 KNQi " +KNOb
100 gms. aqueous solution, simultaneously saturated with potassium and
sodium oxalates, contain 26.15 gms. KsdOi + 2.44 gms. NasCiOt at 25**.
(Foote and Andxew, xgos).
POTASSIUM TeUuric Acid OXALATE Ki[H«TeO..C,04].
Solubility in Water. (Rosenheim and Weinheber, xQxo-xiO
f 0° 20** 30** 40"* so"*'
Gms. Es[H6TeOe.C]04l per 100 gms. HsO 2.67 5.36 6.82 9.07 12.35
POTASSIUM PERMANQANATE KMnO«.
Solubility in Water. (Baxter, Boybton, and Hubbard, 1906; Patterson, X906.)
f.
*.
xoo:
f.
Gms.KMn04
per xoo:
Gms. Solution.
Gms. H,0.
cc. Solution (P).
Gms. Solution.
Gms. HA
0
2.7s
2.83
2.84
34.8
9.64
10.67
9.8
4.13
4.31
• • •
40
II. 16
12.56
IS
« « •
• • ■
$.22
45
12.73
14.58
19.8
S.96
6.34
• • •
SO
14.45
16.89
24.8
7.06
7.59
• • •
SS
16.20
19.33
29.8
8.28
903
8.69
6$
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, X906.)
Aqueous Acetone Solutions at 13^.
(Hers and Knoch, X904.)
Gms. KMnOi per xoo Gms.
cc. Acettme KMnOi per xoo oc. Solution.
f.
/ *-
Solution.
Water.
Solid Phase.
per 100 cc
Solvent.
, «-
Millimah.
Grams.
- 0.18
0.58
0.58
Ice
0
148.5
4.70
— 0.27
0.99
1. 01
M
10
162.5
S.13
— 0.48
1.98
2.02
i(
20
177.3
5.61
- 0.58
2.91
3
ke+KMnO
30
208.2
6.59
+10
4.01
4.22
KMnOi
40
257.4
8.14
15
4-95
5.20
H
SO
289.7
9.16
25
7
7.53
H
60
316.8
X0.02
40
10.40
11. 61
M
70
328
10.38
so
1435
"6.75
M
80
90
XOO
312. 5
227
67
9.89
7.18
2.14
553 POTASSIUM PSBMAN-
QANATE
SOLUBILITT OF POTASSIUM PERMANGANATE IN AqUBOUS SOLUTIONS OF
Potassium Carbonate.
(Sackur and Taegener, 19x2.)
Mob. KMn04 per Liter in:
f.
O.X ff iK«C0^.
X n iKtCO..
a fi iKtCO^.
4 n iK,C0i.
6 n iK,C0k.
0
0.1462
0.0629
0.0446
0.027
0.0156
25
0.4375
0.2589
• • •
0.093
• • •
40
0.7380
0.5007
0.3519
• • •
• • •
Solubility of Potassium Permanganate in Aqueous Solutions of
Potassium Chloride.
(Sackur and Taegener, x9xa.)
Mob. KMn0«
per liter in:
f.
O.Z n KCl.
0.5 n KCL
X n KCl.
3 n KCl.
0
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 Ta^iener, 191 a.)
Mob. KMnOi per Liter in:
V.
H,0.
z n KOH.
a n KOH.
4 n KOH.
6 n KOH.
8 H KOH.
zo n KOH.
0
0.176
0.050
0.031
0.027
0.023
0.017
0.012
10
0.278
0.II2
0.068
0.048
0.042
0.028
0.016
20
O.411
0.179
0.II9
0.079
0.074(x9')
0.032
0.029
30
0.573
0.316(32")
0.213 (32')
0.149(32')
0.II4
0.062(32")
0.040
40
0.792
0.439
0.306
0.2II
O.161
0.084
0.052
so
1. 154(53')
0.638
0.462
0.304
0.219
O.III
• ■ ■
70
1. 812
1. 172
0.869
0.572
0.390
0.188
0.082
80
• • •
I. 513
1. 190
■ • •
0.500
0.231
• • •
90
• • •
• • •
• • •
• • •
0.649
0.297
• • •
Solubility of Potassium Manganate in Aqueous Solutions of
Potassium Hydroxide.
(Sackur and Ta^;ener, 19x2.)
(The KsMnOf was prepared by boiling KMnO^ with very cone. KOH, draining
by suction and washing with ice cold KsCOi solution. The impurities were o?
no consequence since the determinations were made in alkaline solutions.)
Mols. K3Mn04 per
Liter in:
f.
a H KOH.
4 n KOH.
6 n KOH.
8 H KOH.
xo fi KOH.
0
0.907
0.554
0.15s
0.063
0.0145
10
1. 013
• • •
• ■ •
0.070
0.0152
15
• • •
0.681(17")
0.224
• • •
• • •
20
1. 140
0.733(25')
0. 261 (aj")
0.078
0.0160
30
1.252
0.772
0.303
0.096
0.0215
40
• • •
0.852
0.362
0.II9
0.0305
45
1.424
0.889
0.388
• • •
• • •
50
• • •
0.938(51")
• ■ ■
0.142
0.0462
60
• . •
1. 003
0.469
0.167
0.062 (63")
70
• . •
1.074
0.528
0.196
0.070
80
...
I- 143
0.587
0.222
0.083
100 cc. anhy. hydrazine dissolve 2 gms. KMnOi, with evolution of gas and for-
mation of a brown precipitate, at room temp. (Welsh and BioderMn, x9zs.)
POTASSIUM PKRMAN-
QANATE
554
Solubility
OP Mixed Crystals op Potassium Permanganate and
P0TA3SIUM PeRCHLORATE AT 7*".
(Muthmann and Kuotze, 1894; recalculated by Fock, 1897.)
Mol. percent
KMnOiin
Ciyttals of Solid
Phase.
MilUgxam Mols.
per Liter.
KC10>.
0
63.91
29.37
54.48
67.73
42.75
79.04
39.59
99.81
38.63
122.24
34.39
119. 21
38.91
128.08
33.77
144.46
33-14
167.81
29.53
183.09
25.19
197.82
20.16
233 . 75
28.26
264.27
0
Gms. per Liter.
KMnOi.
O
4.65
10.71
12.50
15.79
19.34
18.84
20.26
22.86
26.55
28.97
31.30
36.98
41.81
KCK)«.
8.86
55
7
5
5
5
4
5
4
4
4
3
2
3
o
93
49
36
77
39
68
59
09
49
80
92
o
3.84
9.78
10. 8z
15.96
23.56
24.28
26.40
34.32
44.42
67.33
77.95
94.37
100
Solubility of Mixed Crystals of Potassium Permanganate and
Rubidium Permanganate at f
(Muthmann and Kuntze, calc by Fock.)
Milligram Mols. per Liter.
KMnO«.
Gms. per Liter.
27.04
75
120.26
188.30
198.36
205.76
225.12
264.27
RbMn04.
22.69
22.22
31.29
38.98
41.29
42.50
26
O
KMnOi.
4.28
11.84
19.03
29.80
31.39
32.56
35.61
41.81
RbMnQ«.
4.64
4.54
6.40
7.97
8.44
8.69
5.32
O
Mol. percent
KMnain
Crystals ot Solid
Phase.
3.50
13.75
34.29
71-45
92.50
99.47
99-32
100
POTASSIUM PIC&ATE CeH,(N03)iOK.
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.H1PO4, in Water.
(Parravano and Mieli, 1908.)
Determinations by Synthetic (sealed tube) Method.
Gms.
Gms.
f.
KH,P04.H,P04
per zoo Gms.
Sat. Sol.
SoUd Phase.
f.
KH,P04.H,P04
per xoo Gms.
Sat. Sol.
SoUd Phase.
-0.6
3.337
Ice
65.2
68.44
KHOK)!
-2.5
12.13
M
78
72.43
If
-6.7
29.43
. ««
87. s
77.6
II
- 9.2
36.98
II
105. s
85.9
If
— 13 Eutec.
44 •
" +KH,P04
120 tr.
pt.
92.1
" +KH«PO|.H«PO|
o(?)
45. 8
KH»P04
13s
96.1
KH,P04.H|P0«
+ 10.9
SO. 3
if
139
100
One liter of sat. aq. solution contains 249.9 gms. KHtPO^ at 7^.
(Muthmann and Kontae, 2894.)
555 POTASSIUM PHOSPHATES
Solubility of Potassium Acid Phosphate, KH1PO4.HJPO4, in Anhydrous
Phosphoric Acid.
(Parravano and Midi, 1908.)
Determinations by Synthetic (sealed tube) Method.
Cms. per xoo Gms. Sat. Solution.
V.
KHO'Oi.HtPOi -
KH,PO«.
38. S
18.17
10.56
84
58.42
33-97
no
77-53
45 -08
126. s
92.26
51-90
Equilibrium in thb System Potassium Hydroxide, Phosphoric Acid,
Water at 25®.
(D'Ans and Schieiner, xgxoa; Parker, 19x4.)
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.
Mob. per 1000 Gms. Sat. Sol. „ ,. , «, Mob. per 1000 Gms. Sat. Sol. „ ,. , ^.
K. " PO. - ^^^^ — ns: ' PoT— SohdPhaM.
9
9
9
8
7
8
7
8
9
9
8
8
7
62 O K0H.3H^ 7 4 Ka>04+S:tHP0«
76 0.24 " +K,P04.3H^ 6 3.6 E|HPO«
15 0.5 K.P0..3Hrf) 5 3.15
2 1" 4 2.65 " orKHtPO«(?)
S 1.5 " 3 2.2 " « (?)
2 2" 2 1.7 " " (?)
5 2.5 « 1.5 1. 5 " « (?)
8 2.9 " 1.6 2 KH,PO«
7 2.9 " +K«P04 2.1 4
5 3 ^J^ 2.5 6
5 3-4" 3 8
3.6 " 1.65 6 KHiP04.HaK)4 (Parker)
3-75 " 1-35 8
M M
Fusion-point data for KPOi + K4PSO7 are given by Parravano and Calcagni
(1968, 1910).
POTASSIUM HYPOPHOSPHATE, etc.
Solubility in Water.
(Salzer — LieUg's Aon. axx, x. 82.)
Gms. Saltper too
Salt. Formula. Gms. HsO.
cSd! " SSt.
Potassium Hypophosphate K4P,Oe.8H,0 400
" Hydrogen Hypophosphate K,HP,Oa.3H20 200
" Di Hydrogen Hypophosphate K5ljP,Oe.3H,0 33 100
" Tri Hydrogen Hypophosphate KHJP,Oc 66.6 200
" Penta Hydrogen Hypophosphate K35(P20e)a.2HaO 40 125
" Hydrogen Phosphite KH,PO, 172 (20°)
•' Hypophosphite KH,PO, 200(25°) 333
« Hypophosphite KHJPO,* 14.3(25'*) 28
^ Solvent alcohol.
POTASSIUM PHOSPHOMOLYBDATE K.P04.iiMo0..i}HsO.
100 gms. HsO dissolve 0.0007 PP- ^^ 3^**-
100 gms. aqueous 10% HNOs dissolve 0.204 S^* ^t 30^ (Dook. M. G., 1905.)
POTASSIUM SELINATE 556
POTASSIUM SELINATE K,SeO«.
Solubility in Water.
f. -20". -S*. +5*. i8». 97'.
Gms.KsSe04 per 100 gms. solution 51.5 51.7 52 52.6 54.9
(Etard, 1894.)
100 gms. HsO dissolve 115 gms. KsSeOt at 12°. (Tuttoo, 1907.)
POTASSIUM SILICATE KtSiO,.
Data for equilibrium in the systems KtSiOs + HsO, KsSisOt + HsO, KsSiOs +
SiOj, SiOi + H«0 and KsSiOs + SiOj + HjO, at temperatures between 200* and
1000** +1 determined by the " hydrothermal quenching method/' are given by
Morey (191 7).
POTASSIUM STANNATE K,SnOs.3HsO.
100 gms. HiO dissolve 106.6 gms. at lo^ and 110.5 gms. at 20^ Sp. Gr. at
10® =s 1. 618 at 20° = 1.627. (Ordway, 1865.)
POTASSIUM SULFATE K1SO4.
Solubility in Water.
(Mulder; Aodne, 1884; Trevor, 1891; Tilden and Shenstooe, 1884; Beikd^, 1904; tee also Etard, 1894.)
Gms. K«SO« per 100 Gms. Gms. 'KtSO^ per 100 Gms. Gms. K|SO« per loo Gms.
Water. Solution. Water. Solution. Water. Solution.
o 7.35 6.85 40 14.76 12.86 90 22.8 18.57
10 9.22 8.44 50 16.50 14.16 ibo 24.1 19.42
20 II. II 10 60 18.17 15*38 120 26.5 20.94
25 12.04 10.7s 70 1975 16.49 M3 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:
f.
Sp. Gr. of Sat.
Solution.
Gms. KsSOi per
zoo Gms. HjO.
r.
Sp. Gr. of Sat.
Solution.
Gms.K«S04per
zoo Gms. H^.
0.40
' 1.0589
7-47
58-95
I. 1089
18.01
15 70
1.0770
10.37
74-85
i-"57
20.64
31-45
I. 0921
13 -34
89.70
I "94
22.80
42.75
I . lOIO
1551
loi . I b.
pt.
I. 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
Grams
per Liter.
Sulfate at 25**.
(Fock, Z897.)
Milligram Mols. per Liter. Mol.pcrcent
K,S04. (NH4)sS04. ' ^Kriin*?
734 00 100
778.5 874.6 47.1
483 2126 18.5
340 2685 I I. 13
231 3650 5-9^
0.0 4100 0.00
Sp. Gr.
of
Solution.
1.086
1. 149
1.200
1.226
1.246
1-245
Mol. per oeOi
KsSOtia
SolidPhase.
100
91.28
80.05
68.63
27-53
0.00
K^S04.
127.9
135-7
84.20
59.28
40.27
000
(NH4)sS04.
0.0
"5-7
281. 1
355 0
482.7
542.3
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®.
(Ginrd, 1885.)
Gms. NHs per 100 cc. solution o 6.086 15 .37 24.69 31 .02
Gms. K8SO4 per 100 cc. solution 10.80 4.10 0.83 0.14 0.04
One liter sat. solution in water contains 105.7 ff^^ K1SO4 at 20".
One liter sat. solution in 5.2% NHs contains 45.2 gms. K1SO4 at 20®.
(Konowdow, 1899b.)
Solubility Data for the Reciprocal Salt Pair
K1SO4 + BaCO, T± KiCO, + BaSOi.
(Meyerhoffer, 1905.)
Gn».i)cr
Sat.
too Gms.
Gma-per
xooGmi.
r.
Sol.
SoUdPhue.
f.
Sol.
Solid PhAK.
1C«S04.
KtCO;.
K.SO4.
K.C0,.
25
10.76
0
KtS04+BaS04
25
0.602
7-35
BaCOi+BaSOi
25
6.76
5.85
H «*
25
0.173
2.85
II
25
392
12.6
II •(
80
0.613
2.49
u
25
2.48s
17.81
"+BaC0|
80
1-39
4.88
II
25
1.72
22.1
EiS04+BaC0|
80
71
15-33
"+KtSOi
25
0.0886
28. s
u «•
100
0.797
2.36
BaCOk+BaSOi
25
0.023
53-1
" +KtC0i.aHi0
100
1.83
451
fi **
25
0
53-2
KtCOi-aHflO+BaCO,
100
9.42
13-6
" +K.SO.
Solubility of Mixed Crystals of Potassium Copper Sulfate and
Ammonium Copper Sulfate in Water.
CuS04.K.S04.6H,0 and CuSOiCNHOiSO^.aHjO at 13^-14*
Mol. per cent K Salt.
Mols. per zoo Mols.
H,0-
K. Salt. NH4Salt.
o 1.035
0.0897 0.8618
0.2269 0.6490
0.2570 0.5887
in Solution, in Solid.
O O
5.06 10.34
16.76 33.05
30.40 46.22
Mob. per zoo Mols.
Hfi.
f"55t; NH« Salt.
0.2946 0.5096
0.3339 0.3319
0.4560 O.I961
0.4374 O
(Fock, X897.)
Mol. per cent K Salt.
in Solution, (in Solid.
36.63 58.20
50.15 75-34
69-93 83.86
100 100
Solubility of Some Potassium Double Sulfates in Water at 25^
(Locke, z9oa.)
Double Salt.
Potassium Cobalt Sulfate
Copper
Nickel
Zinc
«
it
ti
ct
Formula.
K2Co(S04)2.6H20
K2Cu(S04)2.6H20
K2Ni(S04)2.6H20
KsZn(S04)2.6H30
Gms. Anhydrous Salt
per zoo urns. H^.
nyc
Gr
12.88
11.69
6.88
13-19
Solubility of Potassium Nickel Sulfate and also of Potassium Zinc
Sulfate in Water, Each Separately Determined at Different Tem-
peratures.
Gms. per zoo Gms. H^.
Gms. per zoo Gms. H|0.
f.
KaNi(S04)t K|Zn(S04)s
.6H^. .6H^.
f.
■•^«'>' "^^"^
0
6 13
40
23 45
10
9 19
50
28 56
20
14 26
60
35 72
25
16 30
70
43 88
30
18 35
POTASSIUM SULFATE 558
Solubility of the Three Hydrates of Potassium Ferrosulfatb
IN Water at Different Temperatures.
(KQster and Thid, x899-)
K|S04.FeS04
^HsO.
K9SO4.FeSO4.4HsO.
N/xoKMn04 Gnu.KaSO/
KsS04.FeS0
t-aHsO.
f.
a:.N/ioKMn6«
Gms. KsSC>4 GC
cc. N/ zo KMnOc Gms. KaSd
jwr ace.
SolutioQ.
JeSOi per
100 cc. Sol.
ner a cc.
Solution.
JeS04 per
xoo cc. Sol.
per 9 cc.
Solution.
JeS04Per.
100 cc. Sol.*
OS
12.4
18.36
15s
22.94
15-4
22.79
17.2
17.0
25.16
18. 1
26.79
21.6
31 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
2;-3
40 46
28.6
42.34
90
• • •
» . «
29.6
43 82
28.9
42.73
95
• • •
• • •
29.8
44.11
27.7
41 .oz
Solubility of Mixtures of Potassium and Lead Sulfates and of
Potassium and Strontium Sulfates in Water.
' (Bane, 1909.)
Results for KsSOi + PbSOi. Results for K1SO4 + SrSOi.
f.
Gms. E^4
per 100 Gms.
Sat. Sol.
Solid Phase.
f.
Gms. KmOi
per xoo Gms.
Sat. Sol.
Solid Phase.
7
0.56
PbS04.E:iS04
17. 5
1.27
KiSO«.SrSO4+SrS0i
17
0.62
• u
50
1.88
M
50
1.09
u
75
2.71
M
75
1-37
u
100
390
m
100
1.69
tt
Solubility of Potassium Sulfate in Aqueous Solutions Of Potassium
Chloride, Bromide, and Iodide.
(Blarez, 1891.)
Interpolated from the original results.
Gfams Halosen
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 Schieiner, 19x0.)
Gnuns KaS04 per xoo cc.
in Aq.
Solutions of:
Ka
KBr
KI
at xa.5*.
at 14*'.
at 13.^.
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
xoooGms.
Gms. per xoo Gms.
Mols. per xooo Gms.
Gms. per xoo Gms.
Sat.l
Solution.
Sat. Solution.
Sat. Solution.
Sat. Solution.
(KOH),.
K,S04.'
KOH. KfSOi.
(KOH),. K«SO«.
' KOH. K|SO«.'
0
0.617
0 10.7s
2.86 0.035
32.06 0.61
0.258
0.433
2.892 7.544
3.42 0.009
38.33 0.16
0-433
0.280
4.854 4.878
4.809 0
53.51 0
1.13
0.137
12.67 2.386
559
POTASSIUM SULFATE
Solubility of Mixed Crystals of Potassium Sulfate and Potassium
Chromate at 25*
' CFock,i897.)
iiUigram
Mols. per liter.
Grams per Liter.
KaSOi. KaCr04l
MoL per cent
KS04m
SdutioQ.
Sp. Gr.
of
Solution.
Mol. per oenf
KsS04iii
SoHd Phase.
' K»SO«.
KaCrO«.
6x8. 1
0.0
107.7
0.00
100. 0
1.083
100. 0
608.4
103
106.0
20.02
85-51
I 092
99-65
341.0
691.8
59-46
134.5
33-01
1. 141
97-30
174.8
1496.0
30 -47
290.5
10.50
1.231
91.97
110. 7
2523
19.30
4905
4.21
I 356
28.43
100.6
2687
17 -54
522.3
3.60
1-377
2.41
0.0
2847
0.0
553-5
0.00
1.398
0.00
734 0
0.0
127.9
0.0
100. 0
1.0863
100. 0
617.0
103.4
107.6
20.1
85-65
1.0934
99.78
463
452.7
80.72
88.0
55-55
I "35
98.49
279
948.2
48.64
184.4
22.72
1. 1700
96.07
153
1469
26.68
285.6
9.41
1-2255
85-77
296
2681
51.61
521.2
21.09
1 .3688
25 -73
0.0
2715
0.00
5278
0.00
I .3781
0.00
Solubility of Potassium Sodium Sulfates in Water.
Double Salt.
f.
uxns. per 100
Gms. H^.
Authority.
3K2S04.Na2S04
103.5
40.8
(Penny. 1855.)
5K4S04.Na2S04
4.4
9.2
(Gladstone, x854*)
«
12.7
10. 1
tt
100
25
Solubility of Potassium Sulfate in Aqueous Solutions of Sodium
Sulfate.
Results at 25^.
(Smith and Ball, 19x7.)
Gms. per xoo Qaa.
HJO.
Na«S0«. K«S04.
O
1.78
3.58
5.38
7.19
12.05
12.33
12.65
12.89
13.12
Results at 34^ and at 60*
(Nacken, 19x0.)
Gms. per xoo Gms.
Sat. Sol. at 34**.
Na9S0«.
O
31.4
33-1
K4SO«.
II. 9
10.7
4.3
o
Gms. per xoo CSms.
Sat. Sol. at 60*.
Na<S04.
O
6.6
27.1
31-3
K«S04.
15.3
13-9
8.2
o
Solid Phase
at 54" and at 6o^
K.SO4
" +Glaserite
Na^i-f Mix oystab
Nai30«
Additional data for the above system at 15*, 25®, 40®, 50*, 60®, 70* and So* are
given by Okada (1914)* The results show that potassium and sodium sulfates
form a double salt of the composition'KsNaCSOi)*. 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 I8^
(Stortenbcckcr, 190a.)
Mols.
KtSO.
xooMds.
K,S04.
1. 10
1-59
2.49
2.75
2-75
2.83
H,S04.
O
0.95
2.70
3-17
3.74
S.08
Solid Phue.
KtSO«
M
K,S0«.KHS0«
11
Mols. per xoo Mols.
K,S04+HjS04+H,0.
K«S04.
2.80
2.61
2.25
1.08
0.77
0.44
Htb04.
5- 79
S-6i
6.19
7-94
9.2
22.7
Solid Phase.
EaS0«.3KHS0«
K^4.6KHS0«
" -fKHSOi
KHSO4
u
M
Solubility of Potassium Sulfate in Aqueous Solutions of Sulfuric
Acid at o**.
(D'Ans, 1909a.)
Mob.
£{.
xooo
Gmt.
Mob.
E
xooo
)Gms.
Sol.
Sdid Phase.
tso*.
Sol.
H,S04:
K^«.
H,S04.
0.53
0.37
K.S04
0.61
2.12
Ka+Kb
0.64
0.7s
II
0.54
2.29
Kb
0.74
I.oS
" +K*H(S04X
O.S3
2.30
" +KHSO4
0.73
1. 13
K«H(S04),
0.43
2.48
KHSO4
0.71
1.44
II
0.28
3.04
II
0.69
1.66
u
0.12
4.43
M
0.69
1.88
" +K*
0.09
S.27
l<
Ka and Kb are acid sulfates between KiH(S04}s and KHSO4. Their composi-
tions were not determined.
Solubility of Potassium Sulfate in Aqueous Solutions of Sulfuric
Acid at 25°.
(D'Ans, x909a, 19x3; see also Hers, 1911-ia.)
Mob. per
Sol.
H,S04.
Solid Phase.
Mob. per xooo Gms.
Sat. Sol.
SoUd Phase.
K^4.
K,SO«.
H,so«+so,;
k
1.27
1. 31
K,S04+K|H(S04),
0.250
8.10
KHi(S04)t.H/)
1-33
1.99
K^CSOJi+Ky
0.352
^•i5
II
1.24
2.03
Ky
0.364
8.16
« -f KH,(S04),
1. 13
2.17
II
0.341
8.29
KH,(S0Jt
1.04
2.35
" -fKHSO,
0.322
833
II
1.032
2.345
KHS0«
0.325
8.45
II
0.67
2.83
II
0.346
6.62
M
0.22
4.13
M
0.384
8.57
M
0.15
536
M
0.412
8.71
M
0.583
8.82
M
e:«so«.
H,S04-fSQ|.
0.880
8.65
" +KHSA
0.171
6.42
KHSO«
0.899
8.63
KHSA (unstable)
0.190
6.60
II
0.882
8.70
II
0.266
6.91
" +KH.(S04)s.Hd0
0.561
8.96
II
0.182
7.26
0.365
9.80
M
O.IS7
7.62
0.43
9.78
M
0.167
7.88
0.665
9.80
M
0.201
8
0.937
9.66
M
Ky = an acid sulfate between KiH(S04)s and KHSO4 of which the exact com-
poeition was not determined.
561
POTASSIUM SULFATE
Solubility of Potassium Sulfate in Aqueous Alcohol.
(Genrdin, 2865; Schiff, 1861.)
In Alcohol of Different
Strengths at 15**.
Weight per
In Aq. Alcohol of 0.939
Sp. Gr. = 40 Wt
0.0J9
40
80
60
Gms. K«S04 per xoo
Gms. AlcohoL
0.16
0.21
0.92
reign
cent Alcohol.
10
20
30
40
Gms. KaS04 per xoo
Gms. Sat. SoL
1.46
0.56
0.21
Solubility of Potassium Sulfate in Aqueous Alcohol at 25^
(Fox and Gauge, 19x0.)
Gms. per xoo Gms. Sat. Solutkm.
Gms. per xoo Gms. Sat. Solution.
'K.S04.
CtHiOH.
Hfi.
K,S04.
CH»0H.
HsO.
9.17
I -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, 19x0.)
IN:
Aqueous
Chloral Hydrate Solutions.
Aqueous Glycerol Solutions.
Gms.
per xoo Gms. Sat. Solution.
Gms.
per 100 Gms. Sat. Solution.
K,S04.
CCl,CH(0H)t.
H«0.
K,S04.
(CH,0H),CH0H.
H,0.
913
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
7983
6.47
20.34
73-19
731
13.20
79-49
5.83
24.15
70.02
S.88
22.07
72.05
4.44
33.73
61.83
454
33 IS
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
3S.I8
2.07
57-22
40.71
1.7s
70.28
27.97
1.53
67.94
30.53
1.40
80.36
18.24
0.98
78.18
20.84
1.08
85.26
13.66
0.73
98.28
0.99
Solubility of Potasshtm Sulfate
Aqueous Acetone Solutions.
AT 25° (Fox and Gauge, 1910.) IN:
Aqueous Pyridine Solutions.
Gms
. per xoo Gms. Sat. S
olution.
Gms.
per xoo Gms. Sat.
Solution.
K,S0«.
(CH,),C0.
H«0.
K«S0«.
CH<(CH.CH),>N.
H^.
7.20
4-92
87.88
7.9s
4.23
87.82
5.02
10.06
84.92
4.77
13.90
81.33
2.96
16.23
80.81
2.7s
24.51
72.74
1.50
24.31
74.19
1.47
34.19
64.34
0.47
37.19
62.34
0.4s
46.29
53-26
0.20
46.29
S3. 51
0.12
55. 93
43-95
0.03
62.40
37.57
0.006
75.90
24.09
POTASSIUM SULFATE
562
Solubility of Potassiuh Sulfate
Aqueous Ethylene Glycol Solutions.
Gms. per xoo Gms. Sat. Solvtion.
KtSO..
iCHjauh-
HaO.
9.67
3.16
87.17
7.69
9-79
82.53
S-74
18.47
75-79
357
32. 11
64.32
1.83
49 03
49.14
AT 25° (Fox and Gauge, 191a) IN:
Aqueous Mannitol Solutions.
Cms. per xoo Gms. Sat. Solutioii.
K,S04.
(CHOH)4(CHiOH)t.
H,0. '
10.32
3 20
86.48
9.61
8.3s
82.04
9.19
11.26
79 SS
8.66
14 30
77.04
^•35
17.22
74.43
Solubility of Potassiuh Sulfate at 25* in:
Aq. Sucrose Solutions.
(Fox and Gauge, 19x0.)
Gms. per xoo Gms. Sat. Solution.
Aq. Potassium Acetate Solutions.
(Fox. 1909.)
Gms. per xoo Gms. Sat. Solution.
-*■
K,SO«.
9-65
8.6s
7.42
4.24
CaHflOi;.
956
18. SS
28.16
37 24
47 SS
S7
H,0.
80.79
72.80
64.42
S6.4I
47 24
38.76
EsS04.
6.6s
509
3-99
^3S
1.23
0.39
CH«COOK.
6. II
8.68'
11.29
IS.S9
20.12
29 ^S
H/).
87.24
86.23
84.72
82.06
78.6s
69.66
100 gms. glycerol cfd==i .255 dissolve i .3 1 6 gms. KsS04 at ord. temp. (Vogei, 1867.)
Solubility of Potassium Sulfate in Aqueous Acetic Acid and in
Aqueous Phenol Solutions at 25**.
(Rothmund and Wilsmore, X903.)
In Aq. Acetic Acid.
Mots, per Liter. Grams per Liter.
In Aq. Phenol.
Mols. per Liter. Grams per liter.
CH^COOH.
KaS04.
CHjCOOH
. K9SO4.
CeHsOH.
KsS()4.
CoHsOH.
KaSO«.
0.0
0.6714
0.0
117 .0
0.0
0.6714
0.0
117. 0
0.07
0.6619
4.2
II5-4
0.032
0.6598
3.01
115 .0
0.137
0.6559
8.22
"44
0.064
0.6502
6.02
"3-3
0328
0.6350
19.68
no. 8
0.127
0.6310
11.94
IIO.O
0.578
0.6097
34.68
106.3
0.236
0.6042
22.19
105.3
i.iSi
0.5556
69.06
96.87
0.308
0.5834
28.97
IOI.7
2.183
0.4743
128.58
82.70
0.409
0.5572
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. KsS04 + 219 gms. sugar at 31.25^ or 100
gms. sat. solution contain 3.18 p^s. KsS04 4- 66.74 gms. sugar. (K5hkr. X897.)
100 gms. 95% formic acid dissolve 36.5 gms. ksSD4 at 2i^ (Aschan, 1913O
100 gms. 95% formic acid dissolve 14.6 gms. KHSO4 at 19.3°. **
100 cc. anhydrous hydrazine dissolve 5 gms. KsS04 at room temp.
(Welsh and Broderson, 19x5.)
100 gms. hydroxylaihine dissolve 3.5 gms. K1SO4 at I7-I8^ (de Bruyn, x89s.)
Freezing-point Data (Solubility, see footnote, p. i) Are Given for the
Following Mixtures:
KiSO* + K2WO4.
-h AgiSO*.
+ NaCl.
-f Na2S04.
+ SrSOi.
It
II
II
II
CAmadori, 19x3-)
(Nacken, 1907b.)
(Sackur, x9ix-xa.)
(Jaenecke, X908; Nacken, 1907 (b) (c); Sackur, z9zi-ia).
(Grahmann, 19x3; Calcagni, 19x2, xgxaa.)
t
563 POTASSIUM BiSULFATB
POTASSIUM BiSULFATB KHSO4.
Solubility in Water.
(Kramers, 1854.)
t*. ©•. ao*. 40*. loo*.
Gms. KHSO4 per icx> gms. HaO 36.3 51.4 67.3 121.6
See also p. 560.
POTASSIUM PerSULFATB KsSsOa.
Solubility in Water.
(Tanigi, 1904)
f.
Gms. KfSiOiPer
100 cc. Sat. boL
f.
Gms. K«S,0t per
100 cc Sat. Sol.
f.
Gms. K^A_per
100 cc. Sat. SoL
0
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 HjSOi liberated, according to the equation KsSiOg+HsO
= KsSOi -f H1SO4 4- O. Taru^ also reports that the presence of a number of
sodium and other salts in solution, does not appreciably alter the solubility of
KfSsOg in water.
100 gms. HsO dissolve 1.77 gms. KsS^Os at o®. (Manhall. 1891.)
Solubility of Potassium Persulfate in Saturated Aqueous Salt
Solutions at 12®.
(Pajetta, 1906.)
(An excess of the salt and of KsSsOg was, in each case, added to water and the
mixture stirred at constant temperature for 10 to 20 hours.)
Water alone 3 196 KsS04 0.798
NajS04.ioH20 6. '238 KHSO4 0.336
NaHS04 8.842 KNO, 0.904
NajHP04.i2H20 4.766 K2COS 0.0146
Na2B407.ioH20 3.825 KHCOs 0.317
NaNOs 19.302 MgS04.7H20 2.990
Na,COMoH20 5.682 CaS04.2H20 3.384
NaHCOs 5.042
Additional determinations made with salt solutions of lower concentrations
than saturation, gave the following results at 12.5^.
Gms. Salt per Gms. KtSA Gms. Salt per Gms. KtS|0|
Salt. 100 Gms. per loo Gms. Salt. loo Gms. ■ per zoo Gms.
H«0. Sat. Sol. Ufi. Sat. Sol.
NatCQi 2.304 4.297 NaHS04 5.218 4- 556
NaHCOj 3.652 4.230 NaNOa 3.696 4.613
Na8S04.ioH20 7 4.554 NasHPO* 3.086 4.446
POTASSIUM Ethyl SULFATE K(QH()S04.
Solubility in Water.
(niiogworth and Howard, 1884.)
Gms. K(CtH|)S04
t*. per zoo Gms.
Sat. Sol.
— 14-2 4SOI
o 53.71
+15 62.3s
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 Howaxd, 1884.)
Results for K(CtH«)S04 Results for K(CH,)S04 Results for K(C»Hu)S04
+ HiO. + H«0. + HiO.
s;ii<Sfi-^(CA)S04 Solid s<Si<£fi. K(CH^S04 SoUd SoUdS. K(C.Hu)S04 Sjlid
«.ti«r -P^ ^^ Phaae. T^hZt Pcr 100 Phase. ^iiZr _P« 100 Phaat
«»^*»- Gms.Sol. ^^'^^ Cms. Sol. <=»*»<«• dms.SoL
— 2.2 10 Ice — 2.3 10 loe — 1.9 10 Ice
— 4-9 20 " — 3.6 IS " — 4.3 20 -
— 8.2 30 " — s 20 « — 5.4 24 **
-12.1 40 " - 8 30 " +K(CJHm)SOi
-14.2 45.01 "+K(CA)S04-Ii.8 39.84 " +K(CH^S04- 4.8 2S K(CiHu)S04
— 6 50 K(CiH«)SO« — ii-S 40 K(CH^S0« o 33.44
o 53.71 " o 47.1 " -I-I7-3 59-46 ••
+15 62.3s " -I-12.3 54.8
POTASSIUM Sodium SULFITE KNa.H(SO,),.4HsO*
100 gms. H|0 dissolve 69 gms. of the ^t at 15*^. (Schwicker, Z889O
POTASSIUM SULFONATES
Solubility in Water.
Gms. Anhy-
Salt. t*. drous Salt per Anthority.
100 Gms. UiO.
Potassium Naphthalene Monosulfonate.iHsO 25 8.48* (Witt, 1915.)
" 2 Phenanthrene Monosulfonate.iHiO 20 0.273 (Sandquist, 191a.)
" 3 " « .oHiO 20 0.342
" 10 " " .iHiO 20 0.84
" o Guaiacol Sulfonate (Thiocol) 15-20 16.6 (Squire ft Gaines, 1905.)
• rf - x.oa9
lOOcc. 90 vol. % alcohol dissolve 0.25 gm. thiocol at 15^-20*^. (Squire and Caiaes, 1905.)
POTASSIUM SULFIDE KsS.
Fusion-point data for KiS -f S are given by Thomas and Rule (1917).
POTASSIUM Antimony SULFIDE, see Potassium Sulfoantimonate, p. 500.
POTASSIUM TARTRATE (KsC4H40e)s.H,0.
100 gms. HiO dissolve 138 gms. KiQHiOs at i6.6^ Sp. Gr. of sat. sol. » 1.49.
(Greenish and Smith, 190X.)
POTASSIUM (Bi) TARTRATE (Mono) KHCiHA, Cream of Tartar.
Solubility of Mono Potassium Tartrate in Water.
(Alluaid, Z865; Roeloisen, 1894; Blares, 1892 ; at 30*, Magnanini, 2901 ; at 25*, Noyes and Clement, 1894.)
Gms. KHCL1H4O1 per 100 Gms. EH(LH«Of per 100
t*. Gms. Solution. t*. Gms. Solution.
"N
o 0.30 (R.) 0.32 (A.) 0.3s (B.) 40 0.96 1.3 1.29
10 0.37 0.40 0.42 50 1.25 1.8 1.80
20 0.49 0.53 (M.) 0.60 60 ... 2.4
25 0.58 0.654 (N. and C.) 0.74 80 ... 4.4 ..•
30 0.69 0.9 (A.) 0.89 100 ... 6.5
Solubility of Mono Potassium Tartrate in Aqueous Alcohol at 25*.
(Seidell, 2910.)
Wt. % j^ Gms. KHC4H«0« Wt. % j _* Gms. KHQHfOi
CJLOH J»%. pcrzooGms. C^OH Cat^l per 200 (ims.
insolvent Sat. Sol. *^Sat. Sol. inSolvent. Sat, bol. Sat. SoL
o 1.002 0.649 50 0.912 0.064
10 0.985 0.358 60 0.890 0.043
20 0.970 0.210 80 0.842 0.023
30 0.953 O.I31 92.3 0.807 0.014
40. 0.933 0.087 100 0.789 O.OIO
565
POTASSIUM BiTABT&ATE
Solubility of Mono Potassium Tartrate in Aqueous Alcohol at i8®.
(Paul, 1917.)
Gms. C2H6OH per 100 cc. solvent o 5 8 10
Gms. EIIC4H406 per liter sat. sol. 4 . 903 3 . 58 2 . 94 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, Z8S4.)
Purified tartrate was added in excess to normal solutions of the adds, and, after
shaking, clear i cc. portions of each solution were withdrawn and titrated with
approximately o.i n Ba(OH)t solution; i cc. normal acid requiring 10.63 <^e. of
the Ba(OH)s solution.
Gms.
cc. N/10
Gms.
Gms.
cc. N/io
Cms
Add.
Add
Ba(OH)s KHC«H«06
Add.
Add
Ba(OH)s KHC«H^
tvou*
perxoocc.
per X cc.
Sdudoa.
per 100 cc.
m aTr"M *
per 100 cc.
Solution.
perxcocc
Solvent.
Solution.
Solvent.
SdutioQ*
HNO,
6.31
5.77*
10.21
C35S0,H
11. 0
5.01*
8.87
HQ
3-^S
5- 32
9.42
HO.{CU,)SO^
12.61
5-33
9-43
HBr
8.10
5.38
9-75
cja^scH
15.81
5.25
9.29
m
12.80
5-43
9.61
HCOOH
4.60
0.4S
0.80
H^O,
4.90
3-97
7.03
CH,COOH
6.00
0.27
0.48
HCH,S04
II. 21
558
12.44
CH2CICOOH
9.45
1. 01
1.79
HCJI5S04
12.61
5-41
9.58
C2H5COOH
7.40
0.24
0.42
HCaH^O*
14.01
5"
9.22
C,H,COOH
8.81
0.23
0.41
* The figures in this column show the amount of the Ba<OH)s aolution in excess of that which would
Solubility of Mono Potassium Tartrate (KHC4H4O6) in Aqueous
Solutions of Electrolytes at 25**.
(Noyes and Clement, 1894; Magnanini, 2901.)
Gm. Equiv. per
Gms
.per
Gm. Equiv. per
Gms. per
Electro-
Liter.
Electro- KHC4'
Liter.
Electro-
lyte.
Liter.
Liter.
lyte.
Electro-
KHC4
Electro-
KHQ'
Electro-
KHQ'
lyte.
H40,.
lyte.
. H4O,.
lyte.
H4O,.
lyte.
H4O,.
Ka
0.025
0.0254
1.86
4.788
CHaCOOK
0.05
0.0410
4.91
7.718
u
0.05
0.0196
3.73
3.680
tt
O.IO
0.0504
9.82
9.486
€€
O.IO
0.0133
7.46
2.509
u
0.20
0.0634
19.63
11.930
«
0.20
0.0087
14.92
1.636
KHS04(2o*»)
O.OI
0.0375
1.36
7.06
KQOi
0.025
0.0256
306
4.821
u
0.02
0.0500
2.72
9.41
((
0.05
0.0197
6.13
3-716
ti
O.IO
0.1597
13-62
30.06
«
o.io
0.0138
12.26
2.601
KHC,04* (20**
)o.oi
0.0369
1.28
6.94
((
0.20
0.0097
24.52
1.728
u
0.02
0.0424
2.56
7.98
KBr
0.05
0.0192
5-95
3699
«
O.IO
O.II32
12.82
21.30
«
O.IO
0.0134
II. 91
2-517
HCl
0.013
0.0367
0.45
6.90
((
0.20
0.0087
23.82
1.629
It
0.025
0.0428
0.91
8.06
KT
0.05
0.0196
8.30
3.687
u
0.050
0.0589
1.82
11.09
((
o.io
0.0132
16.61
2.492
NaCl
0.05
0.0376
2.92
7.08
«
0.20
0.0086
33-22
1. 619
It
O.IO
0.0397
5.85
7.48
KNO,
0.05
0.0195
506
3.676
tt
0.20
0.0428
11.70
8.05
it
O.IO
0.0136
10.12
2.551
NaClO,
0.05
0.0382
5.32
7.18
u
0.20
0.0090
20.24
1.696
tt
O.IO
0.0405
10.65
7.63
KsS04
0.05
0.0208
4.36
3.921
«
0.20
0.0446
21.30
8.40
f<
O.IO
0.0147
8.72
2.769
«
0.20
O.OIOO
17-44
1.888
•
POTASSIUM TABTRATB 566
POTASSIUM Sodium TARTRATE. KNa.C4H«Oe4HsO. (RocheUe or Sdg-
nette Salt.)
100 gms. sat. aq. solution contain 36.66 gms. KNaC4H40« at 9.7*^ and 47.97 gms.
at 29.5^. (vant Hoff and Goldacfamidt, 1895.)
100 gms. HtO dissolve 53.53 gms. KNaC^HiO* at 15% Sp. Gr. of sol. = 1.27 13.
(Greenish & Smith, 190Z.)
Solubility of Mixtures op Potassium Tartrate and of Sodium
Tartrate in Water at Several Temperatures.
(van Leeuwen, 1897.)
^ Gms. per 100 Gms. Sat. Sol. ^ ,. . «. .. Gms. per xoo Gms. Sat. Sol. „ .. .».
^ %CAQ.. "Na,C4I.Q,/ Sobd Phase. f. . ^^^ ^^^^ . Sdid Phase.
18 19.2 16.5 KNaCtHA^H^ 26.6 56 4.2 KNaC«HA-4H^+K«T
38 26.6 22.8 " 48.3 51.6 13.2
20.9 II. 8 28 " +N»,T 59.7 44.5 25.3 K,T+Na,T
38 25.8 24.7 " " 80 39.7 34.7
50 3^-7 23.9 "
KsT = KiC4H40e.}HiO. NaiT = Na,C4H40e.2H20.
Solubility of Several Potassium Salts of Tartaric Acids in Water at 20®.
(Schlossberg. 1900.)
<uu v^w^«u Gms. Salt per xoo
^*- Formula. q^ SatVSoL
Potassium Sodium Salt of Racemic Acid KNa(C4H408).3H20 62.84
Potassium Sodium Salt of d Tartaric Acid KNa(C4H408).4HsO 63 . 50
Potassiimi Neutral Inactive Pyrotartrate K2C5H0O6.H2O 56.33
Potassium Neutral Dextropyrotartrate K2C6H6O6 57-62
Solubility of Potassium Sodium Tartrate in Aq. Alcohol S(X.utions at 25®.
(Seidell, xgzo.)
TTt. %
Sat. Sol.
Gms.
KNaCiH«Or^H,0
per zoo Cms. Solvent
in Solvent.
^of
Sat. Sol.
Gms.
KNaCLH<0L
per 100 Gms. S
0
1.310
53-33
SO
0.908
2.40
10
I. 216
41.60
60
0.878
0.90
20
1. 124
26.20
70
0.857
0.30
30
1.034
13.80
80
0.840
0.06
40
0.961
6
100
0.789
trace
POTASSIUM DihydroxyTABT&ATBS KSC4H4O8.HSO and KHC4H408.H,0.
100 gms. HsO dissolve 2.66 g:ms. KSC4H4O8.HSO at o^. (Fenton. 1898.)
100 gms. HjO dissolve 2.70 gms. KHC4H4O8.HJO 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 TELLURATB KsTe04.
100 gms. HsO dissolve 8.82 gms. KiTe04 at &*, 27.53 8^8* ^t 20** and 50.42 gms.
at 30^. (Rosenheim and Weinheber, 19x0-11^)
POTASSIUM TmOCYANATB KSCN.
Solubility in Water.
t*. Gms. KSCN per
zoo Gms. Sat. Sol.
SoUd Phase.
Authority.
— 6.5 16.7
Ice
(ROdorfF. 1873.)
- 9-55 23.1
u
€t
—31.2 Eutec. 50.25
" +KSCN
(Wassilijew, 19x0.)
0 63.9
KSCN
20 68.5
11
(Rlidocff, 1869.)
25 70.5
M
(Foote, 1903.)
567 P0TASSIX7M THZOCTANATB
SOLUBILITT OF MIXTURES OF POTASSIUH ThIOCYANATB AND SiLVBR
Thiocyanate in Water at 25®.
(Foote, 1903.)
Gms. per zoo
Gms. Sdudan.
Mols. per
kSCN.
xoo. Mols. HsO.
AgSCN.'
Solid
KSCN.
a«scn.
Phase.
70.53
• • •
4436
• • •
K.SCN
66.5s
64.47
61.25
58 -34
9 32
10.62
11.76
13-55
51-13
47 ^S
42.07
38 -47
4.19
4.60'
4-72 ,
5 23
KSCN + aKSCN^SCN
Doable Salt.
sKSCN.AgSCN-
53.92% KSCN
53-21
50.68
1753
20.43
33-71
32 52
6.50J
7.67
aKSCNAgSCN+
KSCN^SCN
49-43
32-51
24.68
20.32
18.34
16.41
30.29
12.26
7-77
7-28)
4.05 ^
3 -02^
Double Salt.
KSCNJ\«SCN-
36.9% KSCN
23.86
16.07
7 36
2.90
KSCN AgSCN + AgSCN
Solubility op Potassium Thiocyanate in Acetone, Amyl Alcohol, etc.
In Acetone.
Gms. KSCN per
®. xoo Gms.
(CHa)sCO.
33
58
20.75
20.40
(von Laszcjmski, 1894.)
In Amyl Alcohol.
Gms. KSCN per
t*. xoo Gms.
CsHiiOH.
0.18
13
65
100
133
1-34
2.14
315
In Ethyl Acetate. In Pyridine,
Gms. KSCN per
. t*. xoo Gms.
CbH»N.
o 6.75
20 6.15
58 4-97
97 3-88
115 3-21
Gms. KSCN per
t®. 100 Gms.
CHtCGOCaHs.
o 0.44
14 0.40
79 0.20
Solubility of Potassium Thiocyanate in Pyridine, Determined by
THE Synthetic Method.
(Wagner and Zemer, xgxz.)
f.
Gms. KSCN
per 100 Gms.
Mixture.
-42
0
—42.1
0.5
-42.4
1-33
—42.8
2.4
SoUd
Phase.
f.
Gms. KSCN
per 100 Gms.
Mixture.
CAN
M
(I
— 43.3Eutec. 3.1
about +10 2.2
« +KSCN
KSCN
70-71
II6-II7
172.7
173.8 m. 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
100 gms. anhydrous acetonitrile dissolve 11. 31 gms. KSCN at 18**.
(Naumann and Schier, 19x4.)
Fusion-point data for mixtures of KSCN + NaSCN and KSCN + RbSCN
are Riven by Wrzesnewsky (1912).
POTASSIUM THZOSULFATB
568
POTASSIUM TmOSULFATB KiStOs.
Solubility in Water. (10,1911,1913.)
f.
Gms. KsSA
per xoo Gms.
SoUd Phase.
f.
Cms. K|SA
per 100 Cms.
HaO.
SoUd Phase.
0
96.1
KA0».2H,0
56.1
234.5
KAQi.HjO+3KA0».HiO
17
150.5
3K«SA.5H«0
60
23^ '3
3K,SA.H/)
20
155 -4
II
65
245.8
M
25
165
1.
70
255.2
«
30
175-7
M
75
268
<l
35
202.4
" +KAQi.Hi0
78.3
292
« +KAO1
40
204.7
K«SA.Hj0
80
293.1
K.SA
45
208.6
II
85
298.5
u
50
215.2
<i
90
312
M
55
227.7
M
POTASSIUM Sodium THIOSULPATB KNaS,0,.2HsO.
100 gms. HjO dissolve 213.7 gms. KNaStOs.2HiO (a) at 15*.
100 gms. HsO dissolve 205.3 gms. KNaS20t.2H20 (b) at 15^
P0TASSIUI.3 FluoTTTANATB K,TiF<.H20.
Solubility in Water. (Marignac, 1866.)
t*. o*. 3'. 6'. xo*.
Gms. KjTiFe per 100 gms. H2O 0.55 0.67 0.77 0.91
(Schwicker. 1889.)
u
14 . 20 .
1.04 1.28
(Radan. 1889.)
POTASSIUM VANADATE K^VsOu-sHiO.
TOO gms. H2O dissolve 19.2 gms. at 17.5^
POTASSIUM ZINC VANADATE. KZnV.Oi4.8H,0.
100 gms. H2O dissolve 0.41 gm. of the salt (Radan).
PRASEODYMIUM CHLORIDE PrCl..
Solubility in Water, Aq. Hydrochloric Acid and in Pyrtoinb.
(Matignon, 1906, 1909.)
Solvent. t*. Sp. Gr. Sat. SoL Gms. per 100 Gms. Sat. SoL
Water 13 1.687 50.96 PrCla
Aq. HCl 13 1 .574 41 .05 PrCl8+7.2sHCl
Pyridine room temp. ... 2.1 PrCla
PRASEODYMIUM QLYCOLATE PrsCCsHsG,)..
One liter water dissolves 3.578 gms. PraCCiHaOa)* at 20®. (Jantsch ft GrOnkiaut. 'ia-13.)
PRASEODYMIUM MOLYBDATE Pr,(Mo04)s.
One liter water dissolves 0.0152 gm. PriCMoO^i at 23** and 0.0143 gms. at 75*.
PRASEODYMIUM Double NITRATES
Solubility at 16° in Conc. HNOj of dj^— 1.325. Jantsch, 19x2.)
Gms. Hydrated
Salt. Formula. Salt per xoo oc
Sat. Solution.
Praseodymium Magnesium Nitrate [Pr(N03)«]2Mg8.24H20
Nickel " " ^- "
<l
Cobalt
u
tt
Zinc
((
u
Manganese
u
a
a
<(
Nis
Cos
Zns
Mna
it
it
it
7.70
9.28
12. 99
14.69
23.40
569 PRASEODYBOUM OXALATE
PRASEODTMIXTM OXALATE PnCCOOsioHsO.
One liter HjO dissolves 0.0007^ gm. Prs(Cs04)s at 25^. (Rimbach and Schubert, 1909.)
100 gms. aq, 19.4% HNOj (a = 1.116) dissolve 1.16 gms. Pri(C204)3 at 15**.
(v. Schede, 1899.)
100 gms. aq. 10.2% HNOi (d = 1.063) dissolve 0.50 gin. PrjCCjOOa at I5^
(v. Scheele» 1899.)
PRA8EODYMIX7M Dimethyl PHOSPHATE Pr,[(CH,),P04]6.
100 gms. HsO dissolve 64.1 gm. Prs[(CHt)sP04]6 at 25^ (Moxgan and James, 1914.)
P&ASEODTMIUM SOLVATE Prs(S04)8.
Solubility in Water. (Muthmann and RoUg, 1898.)
Gms. Pr2(SO«)s
per loq Gms.
Solution.
Solid
Phase.
Gms. Pr2(S04)s
per xoo Gms.
O
18
35
55
Water.
16.5 19.8 Pr,(S04)8^H,0 75
12.3 14. 1 •' 85
9.4 10.4
6.6 7.1 " ,95
Solution.
40
I.O
Water.
4.2
1-55
1. 01
Solid
Phase.
Prs(SO«)t.8HsO
Pr3(S04)«.8H90 +
Pr»(S04)«.sH*0
F^S04)8.5H^
PRASEODTMIUM SULFONATES
Solubility in Water.
Piaseodymium Salt of:
Bromomtrobenzene Sulfonic Add
Benzene Sulfonic Add
m Nitrobenzene Sulfonic Add
m ChloTobenzene Sulfonic Acid
Cbloronitrobenzene Sulfonic Add
a Naphthalene Sulfonic Add
1.5 Nitronaphthalene Sulfonic Add
1.6
1.7
«
((
((
Formula.
Pr(CaH«.Br Jf Ok.SOb,x ,4.2)^-
8H,0
Pr(CASO0«-9H/)
Pr[CgH«(N0i)S0,U.6H|0
Pr[CACl.S0,J,.9H,0
Pr(C,H,.SO,JNOi.a,i ,3,6)1^
X4H«0
Pr[CioH7SQ,],.6HiO
Pr(CuHe(N0|)S0,],. 6B/)
.ixH^
Gms.-Anhy«
p^gl A«UK,rlty.
H,0.
6 . 08 (Katz& James, '13.)
<(
11
S5'^
33.9
12.6
25-9
6.1
0.47
0.18
1-3
(Holmbeig, 1907.)
f«
M
it
«
<(
t€
U
PRASEODYBOUM TUNQSTATE PTi(WO,)z.
One liter water dissolves 0.0438 gm. Prj(W04)i at 75*.
PROPIONIC ACID QHtCOOH.
CHitchoock. 1895.)
Solubility in Water, Determined by the Freezing-point Method.
(Faucon, 29x0.)
fo£
Gms. CiHbCOOH
Solidif.
per
xoo Gms. Sol.
- 1-33
4.98
— 2.60
10. II
- 3- 76
15
— 6.10
25
- 7.70
35.28
— 9.20
45 20
— 10.80
55
— 14.20
65.88
Solid Phase.
fo£
SoUdil.
Gms. CHjCOOH ^^ pj^
per xoo Gms. Sol. ^^
Ice
— 17.2
7348 Ice
«
— 21
81.75
<i
— 29.10
86.85
(1
-29.40
87 . 65 « +CH,C00H
If
— 28.30
89.12 CiH,CXX)H
If
— 26.90
92.40
If
-23.90
97.22
If
-19.30
100
Additional data for this system are given by Tsakalatos (1914), Herz (191 7) and
Ball6 (191 o). 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 Acm between Ether and Aqueous Salt
Solutions at I8^ (de KoiosBovsky, zgzi.)
Salt.
Aq. Salt Solution (2 MoU. per Liter). C|H|COOH per xoo cc of :
Cms. Salt per zoo oc Aq. Layer («) . Ether Layer (fO •
NaCl
MgCU
KNO,
KCiH40t
Water alone
11.69
19.05
20.23
22.43
1. 170
0.762
0.567
0.972
1.324
2.30s
2.543
3.135
2.298
2.406
0.50
0.30
0.18
0.42
0.5s
P lodoPBOPIONIC ACID CHsI.CH,.COOH.
One liter sat. solution in water contains 80 gms. CHal CH2COOH at 25^
(Sidgwicfc. Z9ZO.)
One liter sat. solution in i i» aq. sodium /9 iodopropionate contains 126 gms. at
25^. (Sidgwick, Z9ZO.)
P PhenylPBOPIONIC ACID (Hydrocinnamic Acid) CHsCCeHO-CHaCOOH.
Solubility in Water and in Aq. Normal Sodium /9 Phenylpropionate.
(Sidgwick, zgzo.)
SoWent.
Water
I n aq. CH,(C«H,)CH,.COONa
Gms. CH|(CcH|)CH,COOH per Liter Solutkn at:
, • ,
ZZ'. 21"".
4.80 7.5
7.65 172.5 (liquid layers formed)
Solubility of fi Phenylpropionic Acid in Water and in Alcohols.
(Timofeiew, Z894.)
Gms. CH.(CA)-
CHiCOOHper
100 Gms. &t.
Solution.
AloohoL
f.
AloohoL
f.
Gms. CHtCCtHJ
CHtCOOHper
zoo Gms. Sat.
Soluti<».
Water
Methyl Alcohol
«
a
«
it
Ethyl
19
-18.5
-16
o
+19.6
20
-18.5
-16
0.7
55.8
57.6
66.9
82.8
83.8
46
48
Ethyl Alcohol
Propyl Alcohol
u
«
ti
It
Isobutyl Alcohol
+19.6
20
-18.5
-16
+ 19.6
20
19.6
77.2
78.8
35
39
73.4
73.9
67.3
SoLUBiLrrY OF fi Phenylpropionic Acid in Several Solvents.
(Hen and Rathmaon, 19 Z3.)
CH,(C,H,)CH,.COOH CH,(CA)CH,C00H
Solvent. P^^ ¥^' Solvent. pctUUiT.
Mob. Gms.
4.725 709.2
5.430 815. 1
5.019 753.4
Mols. Gms.
Chloroform 5 . 444 817.2 Tetrachloro Ethylene
Carbon Tetrachloride 4.604 691. i Tetrachloro Ethane
Trichloro Ethylene 5. 140 771.6 Pentachloro Ethane
P Phenyl DibromoPBOPIONIC ACID CsH,Brt(C»Hs)COOH.
100 cc. sat. sol. in carbon tetrachloride contain o. 124 g:ni. acid at 26**. (De Jong, z9o9<)
100 cc. sat. sol. in petroleum ether contain 0.072 gm. acid at 26^. *'
PhenylPBOPIOUC ACID C»H,C : C.COOH.
Solubility in Several Solvents. (Hers and Rathmann, 1913.)
Solvent.
CJI,C:C C(X)H
per Liter.
Solvent.
C4IiC:C.C(X)H
per Liter.
Mols. Gms. Mols. Gms.
Chloroform 0.789 115.30 Tetrachloro Ethylene 0.324 4734
Carbon Tetrachloride o. 227 33 . 16 Tetrachloro Ethane o. 718 104. 90
Trichloro Ethylene 0.382 55.82 Pentachloro Ethane 0.410 5991
PROPIONIC ALDEHYDE CsHtCOH.
100 gms. HsO dissolve 16 gms. aldehyde at 20^. (Vanbel, 1899.)
571
PBOPIONiraiLE
PBOPIONITBILE CHsCN.
Solubility in Water.
S3mthetic method used. See Note, p. i6.
Wt. per cent CsHaCN in:
40
50
60
70
80
90
Aq.
Layer.
10.7
II. 6
12.7
14.9
17.6
C»H«CN
Layer.
92.1
88.5
86.1
83.4
80.2
95
100
105
no
113. 1 (crit. temp.) 48.3
(Rothmund, 1898.)
Wt. per
cent CzHsCN in:
Aq.
C2H5CJI
Layer.
Layer.
19.6
78.0
22.4
75-5
26.0
72.1
32.0
66. s
PROPYL AOETATE, But3rrate and Propionate.
Solubility op Each in Aqueous Alcohol Mixtures.
(Bancroft — Phys. Rer. 3» 205, '95, caic. from Pfeiffer.)
cc. HaO Added to Cause Separation * in:
cc. H2O Added to cause Separation* iiu
ec. Alco-
hol in
P. Ace-
A.
P. Buty-
p. Propio-
cc. Alco-
hol in
r- ^
P. Ace-
K^
p. Buty-
p. Propio-
Mixture.
Ute.
rate.
nate.
Mixture.
tate.
rate.
nate.
3
4 50
1. 19
1.58
21
58.71
19.68
87-83
6
10.48
355
4.70
24
00
23.72
33-75
9
17.80
6.13
8.35
30
32.10
47-15
12
26.00
9 OS
12.54
36
41 '55
63.18
15
35-63
12.31
17-15
42
51.60
83-05
18
47 SO
15.90
22.27
48
54
62.40
73 85
107 .46
• • ■
* cc. HaO added to cause the separation <^ a second phase in mixtures of the given amounts of alcohol
and 3 cc. portions dt propyl acetate* butyrate and propionate
Solubility of Propyl Acetate, Formate, and Propionate in Water.
(Tiaube, 1884.)
100 cc. HsO dissolve 1.7 gms. propyl acetate at 22°.
100 cc. HsO dissolve 2.1 gms. propyl formate at 22^.
100 cc. H2O dissolve 0.6 cc. propyl propionate at 25**.
(Bancroft, 1895.)
PROPYL ALCOHOL CHtOH.
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. C1H7OH at —24® and 57.5 gms. at —30**.^ (Bodmer, 1905-06.)
MisciDiLrTY OF Propyl Alcohol with Mixtures of Chloroform and
Water at o**.
(Bonner, 19 10.)
See Notes, pp. 14 and 287.
Composition of Homogeneous Mixtures.
A
, Composition of Homogeneous Mixtures.
r
jms. cu(n«.
Gms. H^.
Gms.
C,H,OH.
Sp. Gr. of
Mixture.
r
Gms. CHCU.
Gms. HjO.
Gms.
CiHtOH.
Sp. Gr. of
Mixture.
0.977
0.023
0.304
1.28
0.500
0.50
1.34
0.97
0.926
0.074
0.631
113
0.394
0.606
1.32
0.98
0.90
O.IO
0.76
I. II
0.293
0.707
1-235
0.96
0.80
0.20
1.06
1.04
0.194
0.806
0.996
095
0.70
0.30
1.20
1. 01
0.097
0.903
0.672
0.97
0.60
0.40
I 30
0.98
0.030
0.97
0.39
0.97
PROPYL ALCOHOL
572
MisciBiLiTY OF Propyl Alcohol at o* with Mixtures op:
Carbon Tetrachloride and Water.
(Bonner, 19x0.)
Compofiition of Homogeneous Mixtures.
Gms. CCI4. Gms. H/).
0.97s 0025
0931
0.90
0.80
0.70
0.60
0.499
0.40
0.30
*0.25
0.194
o. 100
0.013
0.069
O.IO
0.20
0.30
0.40
0.501
0.60
0.70
0.75
0.806
0.90
0.987
Gms.
CHtOH.
0.317
0.536
0.65
0.949
1. 12
20
234
13
1.06
0.912
I
I
I
I
0.68
0.354
See Notes, pp. 14 and 287.
Sp. Gr. of
Mixture.
1.31
1. 17
1. 14
1.07
1.02
0.99
0.98
0.97
0.96
■ • •
0.96
0.96
0.96
Ethyl Bromide and Water.
(Bonner, 1910.)
Composition of Homogeneous Mixtures.
Gms.
CtH^r.
0.941
0.912
0.90
0.80
0.70
0.60
0.491
0.40
0.30
0.20
0.14
O.IO
"0.023
Gms.H|0.
0.039
0.088
O.IO
0.20
0.30
0.40
0.509
0.60
0.70
0.80
0.86
0.90
0.977
Gms.
C»H,OH.
0.367
0.615
0.64
0.8s
I
1.09
1. 124
1. 10
0.90
0.81
0.671
0.56
0.227
Sp. Gr. ol
Mixture.
I. 21
I. II
1. 10
I. OS
1.02
I
0.98
0.97
0.96
0.96
0.96
0.97
0.99
Miscibdlity of Propyl Alcohol at o* with Mixtures of:
Bromobenzene and Water. (Bonner, 19x0.) Bromotoluene and Water. (Bonner, 19x0.)
Composii
Uon of Homogeneous Mi
xtures.
Composition of Homogeneous M
/ <»
Gms. n... 17 r\ Gms.
CH,CH,Br. Gms.HiO. c^I^h.
ixtures.
r
ims. C^HiBr.
Gms. H«0.
Gms.
CHtOH.
Sp. Gr. of
Mixture.
Sp. Gr. of
Mixture.
0.983
0.017
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
I 05
0.70
0.30
0.96
1. 01
0.70
0.30
I. OS
1.02
0.60
0.40
1.07
0.99
0.60
0.40
I. IS
I
0.50
0.50
1. 13
0.97
0.50
0.50
1. 19
0.97
0.40
0.60
1. 13
0.96
0.40
0.60
1. 19
0.97
0.30
0.70
1.03
0.95
0.30
0.70
1.09
0.95
*0.25
0.75
0.97
• • •
0.20
0.80
0.93
0.9s
0.20
0.80
0.90
0.94
O.IO
0.90
0.71
0.96
O.IO
0.90
0.72
0.9s
0.021
0.979
0.457
0.98
0.013
0.987
0.424
0.96
See Notes
, pp. 14 i
and 287.
Distribution of Propyl Alcohcx. between Water and Cotton-seed
Oil at 25**.
(Wzoth and Reid. X916.)
Gms. CsHtOH per xoo cc.:
Gms. CsHtOH per 100 cc.
Oil Layer.
1-447
1.475
1.503
Ratio.
Ratio.
HjO Layer. """ Oil Layer. HtO Layer.
8. 112 5.60 I. 516 10.07 6.64
8.897 ^10 1.576 10.49 6.65
9.809 6.53 1.694 10.41 6.14
Data for systems composed of normal propyl alcohol, water and various in-
organic salts are given by Timmermans, 1907.
PROPYLAMINE CH,.CH,.CH,.NH,.
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 & (see p. 227) and Ua — 233 when expressed in terms of the
Dstwald solubility expression: (Doyer. 1890.)
573
PROPYL AMINBS
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, 19x2.)
Results at 18"*.
Results at 25**.
Results at 32.35*.
Gm. Equiv.
Gm. Equiv.
Gm. Equiv.
Amine.
Amine per Partition
Amine per
Partition
Amine per PartitM»
liter of Aq. Coef .
Liter of Aq.
Coef.
Liter of Aq. Coef.
Layer.
Layer.
Layer.
Propylamine
0.0973 5.434
0.03837
4.470
0.0602 3. 311
(t
0.0928 5.439
0.04300
4.470
0.0578 3.317
Dipropylamine
0.0764 O.I185
0.0722
0.0769
O.OII68 0.05802
* tt
0.0794 o.n88
0.0681
0.0771
O.OII99 0.0579s
Tripropylamine 0.0003 0.003
• • •
• • •
• ■ • • • •
PROPYLAMINE HYDROCHLORIDE a NH,(C,H7).HC1.
100 gms. HsO dissolve 278.2 gms. NHs(CsH7).HCl at 25®. (Peddle and Turner, 1913.)
ICO gms. CHCli dissolve 5.26 gms. NHj(CtH7).HCl at 25^ (Peddk and Turner, 19x3.)
■
DiPROPYL AMINE HYDROCHLORIDE NH(CsH7)t.HCl.
100 gms. HsO dissolve 165.3 g^is. NH (CtH7)2.HCl at 25*. (Peddle and Turner, X913.)
100 gms. CHClt dissolve 47.24 gms. NH(CtH7)a.HCl at 25^ (Peddle and Turner, 19x3.)
PROPYL CHLORIDE,
Bromide, etc.
Solubility in Water.
(Rex, 1906.)
Grams P.
Compound
per xoo Gms. HjO at:
Propyl CompomMl.
^__.. ...
A..
7—%
o*.
lO*.
ao«.
30^.
CHjCHjCH^Cl (normal)
0.376
0.323
0.272
0.277
CHaCHjCH^r
u
0.298
0.263
0.245
0.247
CHaCHjCiy
u
O.II4
0.103
0.107
0.103
(CH,)2CHC1 (iso)
0.440
0363
0.305
0.304
(CH3),rHBr "
0.418
0.365
0.318
0.318
(CH3),rHT "
0.167
0.143
0.140
0.134
PROPYLENE CHt.
Solubility in Water.
(Tban, i86a.)
f.
fi-
«.
0
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 fi and q,
see Ethane, p. 285.
PYRENE CieHio
Solubility in Toluene and in Absolute Alcohol.
100 gms. toluene dissolve 16.54 gms. pyrene at i8^
100 gms. absolute alcohol dissolve 1.37 gms. pyrene at 10" and 3.08 gms. at
b. pt.
PTRZDIHI 574
PTRZDINX CH < (CH.CH), > N.
Solubility in Water, Determined by the Freezing-point Method.
(Avenge carve from results of Pickering (1893) and Baud (1909.)
H ^p^. i£ ^P^ ii &! P^
fi«^<»- Mixture. **=»'>^- Mixture. ^cb^mo. Mixture.
O O Ice —10 58.5 Ice — 60 84 Ice
— I 7.5 " —12.5 62 " — 65 EuteC. 85 "+CiHiN
— 2 17 " —15 64.5 " —60 87 C»H,N
—3 28 " —20 68 " —55 89
-4 37 S " -25 71 « -50 • 92
-S 43 S " -30 73 S " -45 95
—6 48 " —40 78 " —40 97 "
—8 54 " —50 81.5 " —38m.pt. 100
Timmermans (191 2) 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 pjrridine + water mixtures.
Distribution op Pyridine between Water and Benzene.-
At Room Temperature.
(v. GeorKievics, 1915.)
Cms. C|H«Nper
At 25*.
(Uantacfa and Sebaldt, 1899.)
Mols. C|H^ per Liter.
Ratio.
0.339
0.339
25 cc.H^ Layer.
0.0617
0.0958
^
75 cc.CcH« Layer.
0.4733
0.7631
Aq. Layer.
0.00148
0.00076
C«H« Layer.
0.00436
0.00226
0.1549
0.2432
I . 2249
2.0096
0.00038
0.000208
O.OOIIO
0.000546
0.34s
0.381
0.3297
0.723
1. 147
2.6553
S-4IS9
9.878
(at
(at
So^)
O.OOOII2
0.000456
0.000314
0.000274
0.000928 .
0.001088
0.413
0.491
0.289
Distribution op Pyridine between Water and Toluene.
(Hantzsch and Vagt, 1901.)
At 25**. At Various Temperatures.
Mols. C»H»N per Liter.
VatiA
t*
Mols. CiHftN per Liter.
Ratio.
Aq. Layer.
CACH, Layer.
« .
Aq. Layer.
CHiCH, Uyer.
0.0517
O.II29
0.458
0
0.0168
0.0201
0.840
0.0261
0.0559
0.466
10
0.0135
0.0215
0.627
0.0132
0.0275
0.481
20
O.OIII
0.0228
0.529
0.0067
0.0137
0.496
30
0.0108
0.0234
0.461
0.0033
0.0066
0.551
40
O.OIOI
0.0245
O.4II
0.0019
0.0034
0.629
50
0.0096
0.0252
0.380
O.OOII
0.0017
0.647
70
0.0085
0.0263
0.324
0.0007
O.OOIO
0.696
90
0.0082
0.0266
0.307
Data for systems composed of pyridine, water and various inorganic salts are
given by Timmermans, 1907.
Methyl PTRIDINXS
Ddta for the reciprocal solubility of 5 methyl pyridine ^ = /8 picoline) and
water, 2.6 dimethyl pyridine (= 2.6 lutidme) and water, methyl pyridine (■■ r
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, for 24.6 trimethyl pyridine (collidine) and water.
575
PYRIDINE
PYBIDINAMINO SUCCINIC ACIDS.
100 gms. HtO 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^. CLuts. 1910.)
FTBOCATECHOL 0 C«H4(0H)s.
100 gms. HsO dissolve 45.1 gms. CeHiCOH)] at 20^ (Vaubel, 2899.)
100 gms. pyridine dissolve an unlimited amount of C6H4(OH)s at 20*^. (I>ehii,;[9i7.)
100 gms. aq. 50% pyridine dissolve loi + gms. of C«H4(0H;i at 20-25®. "
F.-pt. data for pyrocatechol + resorcinol are given by Jaeger (1907).
FTBOGALLOL C«H«(OH)s i, 2, 3.
Solubility in Water, etc
(U. s. p. vin.)
100 gms. water dissolve 62.5 gms. C6Ha(0H)a at 25^
100 gms. alcohol dissolve 100 gms. CeHaCOH)! at 2^^
100 gms. ether dissolve 90.9 gms. C6Ha(0H)a at 25 .
Dimethyl PYBONE CrH^Oi.
Freezine-point data for mixtures of dimethyl pyrone and each of the following
compoun(&: salicylic acid, o, m, p and a toluic acids and trinitrotoluene are given
by Kendall (1914a). Results for mixtures of dimethyl pyrone and sulfuric acid
are given by ICendall and Carpenter (1914).
QUINHTDBGNE CeH40k.C6H4(OH)s.
Data for the solubility and dissociation of quinhydrone in water at 25® are
given by Luther and Leubner (19 12).
QIONIDINE CioHmNiOs. ?H,0.
Solubility in Several Solvents.
Sohrent.
Water
Water
Ethyl Alcohol (95%)
Ethyl Alcohol
Methyl Alcohol
Benzene
Benzene
Carbon Tetrachloride
Chloroform
Chloroform
Ether (d = 0.72)
Ether sat. with HsO
HjO sat. with Ether
Ethyl Acetate
Pet. Ether (b. pt. S9*-64**)
I vol. C»H60H-|-4 vols. CHCU
I vol. C»H60H-|-4 vols. CeHe
I vol. CH«0H+4 vols. CHCla
I vol. CH«0H+4 vols. CJIa
QUINIDINE SALTS
Gms. C»Hm NA per 100
■
•r.
/ *^
> Authority.
.
Gms. Solvent.
oc. Solvent
■
18-22
0.020
■ • ■
(MQikr. 1903.)
25
• • •
O.OI45
(Scbaefer, 1910.)
20
4
• • ■
(Wherry & Yanovaky, 29x8.)
25
• • •
2.22
(Schaefer, 1913.)
25
• • •
0.66
II
25
* • •
X.19
u
ia-22
2.45
ft • •
(Mailer, 1903.)
18-22
0.557
ft • •
u
ia-22
100+
ft ft ft
«»
25
• • •
25
(Schaefer, 19x3.)
ia-22
0.78
• ft ft
(MOller. 1903.)
18-22
1.63
ft ft ft
II
18-22
0.031
• ft ft
i<
18-22
1.76
ft ft ft
M
18-22
0.024
ft ft ft
<l
25
• • •
33-3
(Schaefer, X9X3.)
25
• • •
12.5
II
25
• • •
25
M
25
• • •
6.6
U
Solubility in Water at 25*
(Schaefer, 19x0.)
Quinidine Salt.
Q. Hydrobromide
Q. Hydrochloride
Q. Hydroiodide
Q. Salicylate
Gms. Salt per
xoo Gms. HiO.
0.526
1. 160
0.082
0.060
(^uinldine Salt.
Q. Sulfate
Q. Tannate
Q. Tartrate
Q. Bitartrate
Gms. Salt per
zoo Gms. H|0.
I 05
0.0477
2.86
0.323
QUiMIDDnS SULFATE
576
S(X.UBZLITY OF QUINIDINB SULFATE IN SEVERAL SOLVENTS AT 25^
(Schaefer, x9i3-)
Solvent.
I vol. CiH*0H+4 vob. CHCli
I vol. CsHcOH+4 vols. CJi«
X vol. CHjOH+4 voU. CHCU
z vol. CHiOH+4 vols. CA
Solvent.
Cms. Q. SuUftte
per loooc
Solvent.
Ethyl Alcohol
Methyl Alcohol
Chloroform
Benzene
5
40
8.33
Insol.
Gms. Q. Sulfate
per xoooc.
Solvent.
33 3
8.33
33 3
20
QUININE C»Hs4NiOt.3HiO.
SOLUBZLITY IN SEVERAL SOLVENTS.
Solvent.
r.
Anhvdrous Qufnine
Gms. per 100.
Gms. 'CC.
Solvent. Solvent.
Hvdrsted
Gms. Solvent.
Water
iS-22
0.051
• • •
0.0574 (MOller, 1903.)
II
25
0.057
0.033
0.065
(U. S. p.; SduieCer, xgxa)
«
80
0.123
...
0.129
(U. S. P.)
Ethyl Alcohol
20
100
...
• • «
(Wherry and Yanovsky, 19x8.)
<4 ((
25
Z66.6
...
Z66.6
(U. S. P.)
« «
25
• • •
1333
• ■ •
(Schaefer, 1913.)
Meth)d Alcohd
20
■ • •
66.6
• • •
.<
Benzene
25
• • •
0.55
0.205
(Schaefer: MOUer, X903.)
K
20
0.5
• • •
(Wberry and Yanoviky, X918O
((
18-22
1-7
• • •
(MQUer, 1903.)
Aniline
20
14.5
• • •
(Scholtz, 1912.)
Carbon Tetrachloride
20
0.54
0.204
(Gorip 1913; MOller, X903.)
Chloroform
25
50-52.6
62.5
(ScJiaefer, 1913; U. S. P.)
41
ia-22
100+
loo-h
(MttUer. 1903.)
Diethylamine
20
57
• • ■
(SchdU, 191 3.)
Ether
25
22.2
76.9
(U. S. P.)
" (i=o.72)
18-22
0.876
1.62
(MUller, 1903.)
" sat. with HjO
18-22
2.8
5.62
M
HaO sat. with Ether
18-22
0.085
0.067
<t
Ethyl Acetate
18-22
24.7
4.65
M
Petroleum Ether (b.
pt. S9°-64^)
Oil of Sesame
18-28
0.021
o.oio
t<
20
• • ■
0.0453
0.053
(Zalai, 1910.)
Glycerol
25
0.633
0.472
(U. S. P.: OssendowBki, 1907.)
Pipcridine
20
119
■ • •
(ScbolU, 19x2.)
Pyridine
20
lOI
• V ■
u
Aq. 50% Pyridine
20-25
59-4
• ■ •
(Dehn, 191 7-)
7.65 gms. H4BO1 per 100 room
t
cc. aq. 50% Glycerol
temp.
20
• • ■
(Baroni and Barlinetto, 191 x.)
15.3 gms. H4BO1 per 100 room
cc. aq. 50% Glycerol
temp.
40
• • •
u
Solubility of Quinine in Benzene, Determined by the Synthetic
(Sealed Tube) Method.
(van Iteraon-Rotgans, 19x4.)
r.
Wt. %
(2umme.
Solid Phase.
f.
(SbbJ. SoUdPh^K..
f.
Wt.%
Quinme.
5-4
0
CA
53-5
4.81
137
80
5.3*
• ■ •
" +
63
6 . 09 Mixed phase,
142
83.04
17
0.72
CsHmNACA
91
30.01 probably a
146
85.26
29
1.48
t<
102
43.4 colloid or sol-
152
87.44
38.5
2.36
It
104.5
45 . 9 ution of hi|(h
158.5
91.4
49
5.22
" unsuble
109
51.8 viscosity.
166
95.02
±70
28.9
M U
130
75.46
* Eutec.
174.7
zoo
SoUdPhaae.
CbHmNA
M
M
(•
577
QUININE
S(X.UBiLiTY OP Quinine in Aqueous Solutions of Caustic Alkalies.
(Doumer and Derauz, 1895.)
Method. — A one per cent solution of quinine sulfate, containing a very
small amount of HCl, 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
t. Hydroxide.
GnM. NH.
per 900 cc.
Cms. Anhydrous
Quinine
Gms. NaOH
per 200 cc.
Gms. Anhydrous
Quinine
Gnu. KOH
per 300 cc.
Gms. Anhydrous
Quinine
Solution.
Dissolved. ,
Solution.
Dissolved.
Solution.
Dissolved.
0.52
0.084
0.007
0.092
0.612
0.088
0.65
0.084
0.012
0.091
1. 512
0.082
4. 59
0.096
0.740
0.090
3-456
0.068
13 08
0.122
2.160
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
17.074
0.021
0.015
Solubility of Quinine Salts in Water.
(Regnault and WiUejean, 1887.)
Salt.
V.
Gms. Salt per
100 Gms. H^.
Salt.
f.
Gms. Salt per
100 Gms. H^.
Brom Hydrate (basic)
14
2.06
Salicylate (basic)
15
0.114
" (neutral)
12
".33
Sulfate "
14
0.139
« tt
14
13.19
tt tt
16
O.IS3
it a
16
14.79
it tt
18
0.160
It tt
15
14.20
" (neutral)
15
8.50
Chlor Hydrate (basic)
12
3.80
tt tt
17
8.90
(( ((
14
4.14
tt tt
18
9.62
(1 tt
15
4.25
Valerate (ba.sic)
12-
16 2.59
Lactate (basic)
15
10.03
tt tt
37
16.18
Solubility of Quinine Salts in Water at 25^
(Schaefer, 1910.)
Salt.
Gms. Salt per
100 Gms. H|0.
Salt.
Gms. Salt per
100 Gms. HiO-
Acetate
2
H3rpophosphite
2.85
Anisol
0.042
Lactate, basic
16.6
Arsenate
0.154
Nitrate
1.43
Benzoate
0.278
Oxalate
0.071
Bihydrobromide
20
Phosphate
0.125
Bihydrodiloride
143 (133)
Picrate
0.029
Bihydrochloride + Urea
100
Quinate
28.6
Bisulfate
11.78
77 (50)
Salicylate
0.048
Chlorhydrosulfate
Sulfate
0.143
Chromate
0.032
Bisulfoguiacolate
200
Citrate
0.121 (0.
083)
Sulfophenate
0.4
Glycerophosphate, basic
0.1178 (insol.)
Urate
0.182
Hydrobromide
^33
Phenylsulfate
0.147
Hydrochloride
4.76
Tartrate
o.ios
Hydroferrocyanide
0.05
Tannate
o.o5(*)
Hydroiodide
0.49
' Insol.
Valerate
1.25
It is pointed out that different values for the solubility may be obtained ae-
pending on the method used for preparing the saturated solution.
Results in parentheses are by Squire and Caines (1905), and are for 15^-20^
instead of 25^.
QUININE SALTS
578
Solubility op Quinine Salts in Several Solvents.
(Pfadips and Palmer, 191 7.)
^W ^A.
Solubility, Parts per zoo Parts Solvent in:
SalL
M. pt.
(unoorr.)
f
CCI«.
CHCU Ethyl Acetate (Alcohol free)
(Alcoholfree). ' Cold.
Hot.
Quinine racemic lactate
165.5
0.00715
28.6 0.286
3-33
d lactate
175
O.OIII
0.2s
/ "
171
0.00476
0.20
formats
IIO-II3
0.00625
acetate
124-126
0.05
propionate
iio-ni
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
183-5
. 0.00167
0.0833
sulfate
214
0.0025
0
0333 0.00715
0.0133
Quintozime lactate
• • •
O.II
1 •
• • •
• • •
Saturation was obtained by shakinff 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 HYDBOCHLOBIDB C»HmNsOs.HC1.2H,0.
Solubility in Aqueous Salt Solutions at 16®.
(Tarugi, 1914-)
The determinations were made bv adding an aqueous solution of quinine
hydrochloride to the aqueous salt solution until turbidity occurred. From the
volumes involved, the solubility per 100 cci was calculated.
In Aq. NaCl.
Gms. per 100 cc. Sol.
NaCl. Q.HCl.'
9.02 2.6
2.49 1.94
3.40 1.22
8.34 0.54
ZI.40 0.205
15.56 0.140
19.83 0.085
In Aq. NaNOi.
Gms. per 100 cc. Sol.
NaNO,. Q.HC1.
0.677 2.85
0.970 X.96
2.008 0.67
3.65 0.43
9.31 0.292
19,12 0.168
31.78 0.0663
In Aq.KCl.
Gms. per 100 cc. Sol.
In Aq. CaClt.
Gms. per xoo cc. Sol.
KCl.
2.63
3
5. 57
8.26
ZO.42
17.87
25 -74
Q.HCl.
2.545
1.882
0.804
0.531
0.407
0.205
0.0997
CaCl,.
6.37
7.03
7.75
7.96
34 42
Q.HC1.
1.028
0.951
0.879
0.765
0.183
II
II
(Squire and
Caines,
1905.)
100 cc. 90% alcohol dissolve 20 gms. Q. bihydrochloride at 15^-20**.
chloroform " 14.3 "
90% alcohol " 14.3 " Q.hydrochloro8ulfateati5®-20®.
" " 0.5 " Q. glycerophosphate at i5*'-20**.
100 gms. HiO dissolve 1.3 gms. anhydrous Q. glycerophosphate at 100".
(Rogier and Fiore, 1913.)
QUININE SALICYLATE C»Hs4NA.GH4(OH)COOH.2HtO.
Solubility in Aqueous Alcohol at 25®.
(Seidell, 1909, 19x0.)
wt. %
diLOH
in Solvent.
dnot
Sat. Sol.
Gms. Q. Sal.
aHjO oer xoo
Gms. ^t. Sci
Wt. %
in Solvent.
^of
Sat. Sol.
Gms. Q. Sal.
aHiO per 100
Gms. ^t. Sol.
0
0.999
0.065
60
0.896
2.45
10
0.982
0.080
70
0.876
3.25
20
0.966
0.200
80
0.854
4.20
30
0.952
0.48
90
0.832
4.71
40
0.935
I
92.3
0.826
4.62
50
0.916
1.70
100
0.797
3.15
579 QUININE SULFATE
Solubility op Quinine Sulfate in Several Solvents at 25**.
(Schaefer, 19x3.)
Q^Urm^* Gm». Q. Sulfate c«i«.«» Gms. Q. Sulfate
Solvent. per loocc Solvent. Solvent. per 100 cc. Solvent.
Ethyl Alcohol 0.4 i vol. CjH»0H-|-4 vols. CHCl* 12.5
Methyl Alcohol 3.12 i vol. CiH»0H-|-4 vols. C^He o . 53
Chloroform 0.27 i vol. CH«OH4-4 vols. CHCU 20
Benzene insol. i vol. CHsOH+4 vols. CeHs 4.76
ioognis.trichlorethylenedissolveo.o7gm.Q.sulfateat 15^ (Wester and Bruins, 1914.)
QUININE TANNATES True and False
Solubility in Water and in Aqueous HCl at 37"*. (Muraro, 1908 J
Cms. Q. Tannate per loo Cms.
Tannate. Formula. * H^. A^^^% Ag.^%
True Tannate I C10Hs4NtOft.C10H14O9.4HsO o 0.984 3.656
True Tannate II (CsoH24NsOi)s.(CioHuOg)s.8H30 o z.210 4.756
False Tannate (CsoHs4NiOt.HsS04)t(CioHuOg)i.i4HsO 0.313 0.847 i-S^o
The work of Muraro is criticized by Biginelli (1908).
100 cc. 90% alcohol dissolve 33.3 gms. Q. tannate at 15^-20°. (Squire and Gaines, 1905.)
QUININE PYBOTABTRATES I, i, d.
Solubilities in Alcohol at i8^ (Ladenburg and Herz, 1898.)
100 gms. alcohol dissolve 15 gms. of the / pyrotartrate, 3.2 gms. of the « 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 f quinine compound is a salt of the racemic acid.
Solubility of Quinine and of Quinine S.\lts in Water and Other
Solvents. (U. s. p. viii.) ■
Cms. Quinine Compound per xoo Gms. Solvent in:
Compound.
CioHsiNtOft
C«Jis4N,0,.3HsO
CsoHs4NsOiHC1.2HsO
C»HiM.NsO,.C«H4(OH).-
COOH.iH,0
(C»H,4N2Q2)».H,S04.7HsO
CsoHmN,0,.H,S04.7H,0
CnHs4NsQ2.HBr.HsO
QUINOLINE ETHIODIDE CsHtN.CHsI.
100 gms. HiO dissolve 301.3 gms. C^HtN-CiHsI at 25*. (Peddle and Turner, 19x3.)
100 gms. CHCli dissolve 1.78 gms. CsHtN.CiHsI at 25°. "
RADIUM EMANATIONS
Solubility in Water. (Bqyle, 1911; Kofler, 19x3.)
Solubility. Solubility.
L\ , '^ ^ f. , * s
/(Boyle). a (Kofler). /(Boyle). a (Kofler).
O 0.508 0.54 30 O.IQS 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 ... O.I2
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
p. 227). Those of Kofler are in terms of the expression a — • -=, where
V lis
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.
Water.
Alcohol.
Ether.
Chloroform.
Glycerol.
'At
as*.
At 8o". '
At as*.
At
as*.
At
as*.
At as*.
0
057
0.123
166.6
22
2
52
.6
0.633
0
.065
0.129
166.6
76
9
62
5
0.472
s
•55
250
166.6
0
417
122
12.2
I
30
2.86
9.09
0
.91
2
■70
6.25
0
139
2.22
1. 16
■ • •
0
25
2.78
II
■77
147
555
0
.056
0
.109
5-55
2
■5
33-3
149.2
6
.2
•
» •
12.5
RADIUM EMANATIONS
580
Solubility in Several Solvents.
(Ramstedt, 19x1; Swinne, 19x3.)
Solvent.
Water
Sea Water
Ethyl Alcohol
Amyl Alcohol
Acetone
Aniline
Benzene
Carbon Disulfide
Chloroform
Cyclohexane
Ethyl Acetate
Ethyl Ether
Glycerol
Hexane
Toluene
8
•
7
4
•
33
20
•
9
20
•
23
18
Results at o*.
1^ Sp. Gr. of SoL
52 0.9999
• • • •
28 0.8065
• ■ V •
99 0.8186
43 I 0379
V • • •
4 I. 2921
5 1.5264
• • • •
41 0.9244
9 0.7362
• • ■ •
4 0.6769
4 o. 8842
Results at 18*.
0.285
• • •
6.17
• ■ •
6.30
3.80
12.82
23 14
15.08
18.04
7.34
1508
0.21
16.56
13.24
Sp. Gr. ofSoL
0.9986
• • •
O.7911
• • •
0.7972
I. 0210
0.881 I
I . 2640
1.4907
0.7306
0.9029
0.7158
1.262
0.6612
0.8666
Results at 14*.
(Boyle, 19x1.)
/u
0.30
0.255
7.34
9.31
13.7
The above results are in terms of the Ostwald Solubility Expression (see p. 227).
BE80B0IN0L GeH^COH), i, 3.
Solubility in:
Water.
Ethyl Alcohol.
(Speyers^
Sp.Gr.of
Am. J. Sd. [4] Z4, 394, '03.)
Gins.CaH4(OH)s per loo Gms.
Sp.Gr.of
(Speyers.)
t^
Gms. C6H4(OH)s per loo Gms. ^
• •
Solutions.
Water. Solution.
Solutions.
Alcohol.
Solution.
0
I.IOI
60 37 5
I 033
210
67.8
10
1. 118
8z 44.8
1.036
223
69.0
20
I 134
103 50 -7
1. 041
236
70 -3
25
1. 142
"7 53-9
1.045
243
70.8
30
1. 148
131 5<^-7
1.048
250
71.4
40
I -157
161 58.9
1.056
266
72.7
50
1.165
198 66.5
1.065
286
74.1
60
1. 172
246 71. I
I 075
3"
75-7
70
1. 176
320 76.2
1.087
341
77-3
80
1. 179
487 82.9
1. 104
375
78.9
Note. — The original results of Speyers are given in terms of mols. per 100
mols. HsO.
According to Vaubel (1895), 100 gms. HjO dissolve 175.5 gn^s. CeHiCOH)!,
or 100 gms. sat. solution contain 63.7 gms. at 20**. Sp. Gr. of sol. » I.i335*
Solubility of Resorcinol in Alcohols and in Acids.
(Timofeiew,
• 1894-)
Gms. C|H«(OH)i m
Gms. CACOH)}
Solvent.
f.
per zoo Gms.
Solvent.
f.
per 100 Gms.
Sat. SoL
•
Sat. Sol.
Methyl Alcohol
11. 6
69
Formic Add
IS
29.2
Ethyl
10.4
59-2
Acetic "
15
32.5
« «
II. 6
61. 5
Propionic "
15
22.8
Propyl "
10.4
51.5
Butyric "
15
14.7
It It
II. 6
51.6
Isobutyric "
IS
9.6
Valeric "
15
6.S
58i USSOBCINOL
Solubility op Rbsorcinol in Benzene.
(Rothmand, 1898.)
r.
Cms. CACOH).
per 100 Gms. Sat. Sol.
f.
Gms. C^HtCOH).
pet 100 Gina. Sat. Sol.
73
3.18
95 S
61.7
77
4-75
96s
77.64
82
6.94
83.46
98. s
9SS
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:
t*
Gms. CtH4(0H)« per zoo Gms.
ft*
Gm. C«Hi(OH)i pet lOo Gnu.
ll .
CA Layer.
CA(OH)i Uyer.
• *
' CeHe Layer. C^HiCOH), Uyer.'
60
4.8
79-4
90
13 71 -3
70
6.6
77-5
100
19s 65.7
80
9.2
75
105
109 -3
24.6 60.7
crit. temp. 42.4
Resorcinol mixes with pyridine in all proportions. (Dehn, 1917.)
1 00 gms. aqueous 50% pyridine dissolve 001 gms. CsH4(0H)i mat 20^-25®. "
loocc. olive oil dissolve 4.55 gms. CsH4(0H)i mat 15^-20**. (Squire and Caincs, 1905.)
The coefficient of distribution of resorcinol at 25® between olive oil and water
(cone, in oil -i- cone, in HsO) 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 Vignon (i8oi).
Results for mixtures of resorcinol and m xylene are given by Campetti (191 7).
Distribution op Resorcinol Between Water and Organic
Solvents at Ordinary Temperature.
(Vaubcl — J. pr". Ch. [a] 67. 478. '03)
Gms. Gms. CeH^COH) in:
C^H^iOBh Solvents.
Used.
1 . 191 60 cc. HjO-h 30 CO. Ether
1 . 191 60 cc. H204- 60 cc. Ether
0.800 40 cc. H2O+ 40 cc. Benzene
o-8oo 40CC. HjO^- 80 cc. Benzene
0.500 50 cc. H204- 50 cc. CCI4
o ■ 500 50 cc. HjG + 100 cc. CCI4
o • 500 50 cc. HjO + 150 cc. CCI4
RHODIUM SALTS. Solubility in Water.
(Jorgenscn — J. pr. Ch. [2] a7. 433. '83; 34t 394. '86; 44, 51, '91.)
Salt. Formula.
Chloro Purpureo Rhodium Chloride ClRh(NH,)5Cl,
Luteo Rhodium Chloride RhCNHJeCl,
Luteo Rhodium Nitrate RhCNH^sCNO,),
Luteo Rhodium Sulphate [Rh(NH,)«t(S04),.5H,0 ao a. 3
HsO Layer.
Organic
Solvent Layer.
0.2014
09896
0.247S
0.9525
05873
02127
0.5773
0.2227
0.4885
0.0x15
0.4880
0.0120
0.4880
0.0120
6; 44. 51. '<
91)
t*
Gms. per 100
w «
Gms.HaO.
17
0.56
8
^3-3
(
Did,
. t 2.1
BOSANnJNE CsoHuNsO.
100 gms. Hj() dissolve 0.03 gm. C^ioHnNiOi at 20*-25**. i
100 gms. pyridine dissolve 41.5 gms. CioH2iNt04 at 20*'-25"*.
100 gms. aq. 50% pyridine di^lve35.i gms. CsoHuNtOi at 2o'*-25°.
(Dehn, 1917.)
B08ANILINK 5^3
Triphenyl p BOSANIUNE HYDBOCHLOBIDK (C«H4.NH.CeHi)tC(0H).HCL
Solubility in Several Solvents at 23**.
(v. Szathmaiy de Szachmar, 1910.)
Solvent. Roeaniline HC
Gms. Triphenyl p
loeaniline HClper
100 Gms. Sat. SoL
Methyl Alcohol 0.447
Ethyl " 0.285
Amyl " o.ii
Acetone o . 19
Aniline 0.518
B080LIC ACID C»Hi«Oa.
100 gins. HsO dissolve 0.12 gm. CwHieOs at 20*^-2g^ (Dehn, 1917.}
100 gms. pyridine dissolve 160 gm. CwHitOi at 20-25°. "
100 gms. aq. 50% pyridine dissolve 80 gm. CsoHieOs at 20^-25^ **
BUBIDIUM ALUMS. See also Alums, p. 32.
Solubility in Water.
(Locke. iQox.)
Gms. Alum per xoo Gms. HjO.
Alum.
t».
Anhydrous.
Hydrated.
G.Mols.
Rb. Aluminum Alum
RbA](SOJ,.i2H,0
25
1. 81
3- IS
0.0059
<i
tt
30
2. 19
• • •
0.0072
ti
K
35
2.66
• ■ •
0.0087
«
tt
40
3.22
* • •
0.0106
Rb. Chromium Alum
RbCr(S04),.i2H,0
«5
2.57
4.34
0.0079
II
tt
30
3- 17
V • •
0.0096
II
tt
35
4. II
• • V
0.0128
41
It
40
5-97
• • •
O.0181
Rb. Vanadium Alum
RbV(S04),.i2H,0
RbFe(S04),.i2H,0
25
5-79
9 93
16.98
0.0177
Rb. Iron Alum
25
9 74
0.0294
((
<c
30
30.24
• ■ •
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.
BUBmiUM FLUOBOBIDB RbBF.
100 gms. H2O dissolve 0.55 gm. RbBFi at 20^ and i gm. at loo^ (Godeffroy, 1876.)
BUBIDIUM BBOBSIDB RbBr.
Solubility in Water.
(Rimharh, 1905.)
Gms. RbBr per 100 Gms. Gms. RbBr per 100 Ums.
V. t -* N f * ->
Water. Solution. Water. Solution.
0.5 89.6 47.26 39.7 131-85 56.87
5 98 49.50 57.5 152.47 60.39
16 104.8 51.17 "35 205.21 67.24
Freezing-point data for RbBr + AgBr are given by Sandonnini (1912a).
BUBIDIUM BiCABBONATE RbHCO,.
100 gms. sat. solution in HsO contain 53.73 gms. RbHCOa at about 20^.
(de Forcrand. 1909O
BUBIDIUM CABBONATE Rb,CO,.
IDG gms. absolute alcohol dissolve 0.74 gm. RbtCOs. (Bwuen.)
583
RUBIDIUM CHLORATE
RUBIDIUM CHLORATE RbClOi.
Solubility in Water.
(Calzolari. x9ia.)
Gtas. RbClO^ per 4«
xoo Gms. afi. * '
2 . 138 42 . 2
3 07 SO
5-36 76
8 99
There is some uncertainty as to whether the results of Calzolari refer to 100
gms. of HtO or 100 gms. of saturated solution.
1 00 gms. HsO dissolve 3 . i gms. RbClOs at 1 5° {di$ of the sat. sol. = i .07) . (Carlaon. 'xa)
For earlier data see Reissig, 1863.
RUBIDIUM PerCHLORATE RbC104.
Solubility in Water.
(Carlson, 19x0; Calzolari, 1912,)
f.
O
8
19.8
30
Gms. RbQCXper
xoo Gms. H^.
12.48
15.98
34.12
62.8
f.
Gms. Rba04 per 100 Gms. H^.
f.
Gms. Rba04 per 100 Gms. H^.
(Carlson.) (Calzolari.)
I.I (1.007) SO 3.5
1.2 60 4.85
1.56 (i.oio) 70 6.72
1.8 80 9.2
2.2 90 12.7
3.26 (1.OI7) 100 18
The figures in parentheses are densities of sat. solutions.
100 gms. HiO dissolve 1.08 gm. RbClOi at 2I.3^
(Calzolari.)
0
O-S
10
0.6
20
I
2S
1.2
30
I-S
40
2.3
(Carlson.)
4.6
6.27 (1.028)
8.2
11.04 (1.050)
IS -5
22 (?) (1.070)
(Longttimine, 1862.)
RUBIDIUM Potassium PerCHLORATE RbtKCClOOa.
IDG gms. sat. solution in HsO contain 1.55 gms. RbtK(C104)i at 20^ (dn of the
sat. solution — 1.013).
((^Ison, X9xa)
RUBIDIUM CHLORIDE
RBCl.
Solubility
in Water.
1
CRimbach, 1903;
Berkeley, 1904.)
t\
Mols.Rba
per liter.
Gms. RbCl
per 100 Gms.
4,0 MolB.Rba
Gms. RbC3
per xoo Gm
Water.
Solution.'
"Water.
Solutica.
0
S17
77 0
43 5
60 6.90
^^5S
53-6
10
sss
84.4
45-8
70 7.12
121. 4
54.8
20
s-88
91. 1
47-7
80 7-33
127.2
56.0
30
6.17
97.6
49.4
90 752
133 I
571
40
6-43
103 s
50-9
100 7.71
138.9
589
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^ 0.55 18.7' 31. 5 ' 44.7 60.25 75. IS 89.35 "4*
Sp. Gr. X.4409 1.4865 1.5118 1.5348 1.5558 15746 1.5905 1. 6148
* Boilmg-point.
100 gms. methyl alcohol dissolve I.41 gms. RbCl at 25^. (Tamer and Bissett, 19x3.)
*^ ethyl " " 0.078 gm. " " "
propyl " " 0.015
amy! " " 0.0025
100 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 + TlCl are given by Sandonnini (191 1. 1914). Results for RbCl + NaCl
are given by Zemcznzny and Rambach (1910}.
«
II
11
II
II
II
II II
II II
M
RUBIDIUM CHLOBIDK 584
RUBIDIUM TELLURIUM CHLOBIDB RbiTeCU.
100 gms. aq. HCl of 1.2 Sp. Gr. dissolve 0.34 gm. RbiTeCU at 23^
100 gms. aq. HCl of 1.05 5p. Gr. dissolve 13.09 gms. RbiTeCU at 23°.
(Wfaeder. 1893.)
RUBIDIUM THALLIUM CHLORIDB 3RbClTlCU.2H«0.
100 gms. HsO dissolve 13.3 gms. at 18°, and 62.5 gms. at 100^. (GodefiEioy. 1886.)
RUBIDIUM CHROMATE (Mono) RbiCr04.
Solubility in Water.
(Schreinemaken and FUippo, Jr., 1906.)
r.
Gms. RbCiOi
per 100 Gms.
Solutkm.
Cms. RbCiO«
V. per zoo Gnu.
Solution.
f.
Gms. RbCi04
per 100 Gms.
Solution.
7
0
10
36.65
38.27
40.23
SO 47.44
60.4 48.90
Solid Phase, Ice
— 2.40
-3.2s
-4.14
IS.S8
20.03
24.28
20
42.42
—0.6 0.95
-s-ss
30. IS
30
40
44.11
46.13
— I.I 7.22
-1.57 9.87
—6.71
about —
34.31
'7 36.65
Equilibrium in the System Rubidium Oxide, Chromium Trioxide and
Water at 30°.
(Schreinemakeia and Filippo, Jr., 1906.)
Gms. per 100
Gms. Sat. SoL
Gms. per zoo Gms. Sat. Sol.
Solid Phase.
Solid Phase.
CtO|.
Rb,0.
CrO,.
Rb,0.
0
60.56
RbOH
13.91
3.38
RbiCrA
0
56.82
RbiCiOi
15.05
3.45
" +Rb,CrK)»
0.776
37-88
u
15.31
3.59
Rb,CrA
2.89
34- 89
<l
15.19
3.19
RbiCrA-!
4.96
30.20
«
18.96
2.37
41
8.54
28.17
II
24.92
1.66
•4
11.98
27.99
II
37.34
1. 61
II
15.38
28.73
II
48.20
1-54
<l
I5S4
28.55
" +Rb,CrA
53.87
1.67
11
13.69
23.87
Rb,CrA
54.29
1.28
" +RbaCr40tt
9.98
17 56
<i
58.69
1.07
Rb|Cr40u
S-72
8.47
II
62.38
0.93
II
4.58
7.98
H
62.74
0.93
II
4.87
4.60
II
63.07
0.92
" +C1O,
8.16
3.57
II
62.28
0
OrOk
RUBIDIUM DICHROBiATE RbtCnOT.
Solubility of the Polymorphic Forms in Water.
(Stortenbecker, Z907; see also Wyrouboff, Z90Z.)
r.
Gms. RbiCr A per loc
> Gms. Sat. Sol.
Monoclinic Form.
Triclinic Form.
18
5.42
4.96
24
6.94
6.5s
30
9.08
8.70
40
13.22
12.90
50
18.94
18.77
65
28.10
27.30
100 gms. sat. aq. solution contain 9.47 gms. RbtCrtOr, at 30^.
(Schreinemaketa and FQippOk J'm x9o6.)
RUBIDIUM FLUORIDB RbF.i^H/).
100 gms. H|0 dissolve 130.6 gms. RbF at i8^
(de Foicrand, 191 zO
585 BUBIDIUM HYDROXIDE
RUBIDIUM HYDROXIDE RbOH.
100 gms. sat. aqueous solution contain 63.39 gms. RbOH at 30*^.
(Schrejnemakers and Filippo,i9o6.)
loop^ms. sat. aqueous solution contain 64.17 gms. RbOH at 15°. (de Forcrand, z9o9a.)
Fusion-point data for mixtures of RbOH + NaOH are given by (v. Hevesy,
1900}.
RUBIDIUM lODATE RblO,.
100 gms. H|0 dissolve 2.1 gms. RblOi at 23°. (Wheder, 1893.)
RUBIDIUM PerlODATE RbI04.
100 gms. HsO ciissbtve~o.65 gm. RbI04 at 13**, diM of sat. solution — 1.0052.
(Barker. 1908.)
RUBIDIUM IODIDE Rbl.
100 gms. HfO dissolve 137.5 gms. Rbl at 6.9^ and 152 gms at I7.4^
(Reissig, 1863.)
Solubility of Rubidium Iodide in Organic Solvents.
(Walden, 1906.)
Solvent.
Formula.
CHjCN
CjHsCN
(CH,),CO
C4H,0.C0H
ir Rbl + Agl are
Gnu. Rbl per loo cc Solution.
*
Acetonitrile
Propionitrile
Nitromethane
Acetone
Furfurol
Fusion-point data fc
1.478 at o"* 1.350 at 25**
0.274 " 0.305 "
0.567 " 0.518 "
0.960 " 0.674 "
4.930 "
given by Sandonnini (1912a).
RUBIDIUM PerlODIDES
Solubility in Water at 25".
(Foote and Chalker. 1908.)
Rbl.
I.
Sotid Phase.
Rbl.
1.
SoUd Phase.
61.93
0
Rbl
28.01
64.85
Rbla+I
59-94
S-90
" +RbI,
27.8s
65.12
II
57-24
8.02
Rbl,
27.83
65.13
i<
33-89
38.08
II
27.99
64.98
<4
The results shdw that Rbl? and Rbl» are not formed.
RUBIDIUM BROMIODIDE RbBrJ.
100 gms. sat. aq. solution contain about 44 gms. RbBril, and the Sp. Gr. of
the solution is 3.84. (Wells and Wheeler, 1899.)
RUBIDIUM ntlDATE and IRIDITE8
Solubilities in Water.
(DeKpine, 1908.)
Salt. Formula. f. Gm^^^^,
Rubidium Chloroiridate Rb2lrCl6 19 o.oSSS
Trirubidium Hexachloroiridite RbsIrCU.HsG 19 0.91
Dirubidium Aquopentachloroiridite Rb2lrCU(HjO) 19 1.05
RUBIDIUM ParaMOLYBDATE 5Rbs0.i2MoO,.H,0.
100 cc. sat. aq. solution contain 1.941 gms. of the salt at 24*^. (Wempe, 1912.)
RUBIDIUM NIT&ATK 586
RUBIDIUM NTTRATK RbNQi.
SOLUBILITT IN WaTBR.
(Berkeley, 1904)
*•
Mols.
RbNOi
Per Liter.
Grams RbNQi per xoo Gms.
f.
Mols.
RbNOi
Per Liter.
Cms. RbNOtj>er xoo Gnm
B .
Water. Sdutian.
Water. Solution.
0
1.27
19.5 16.3
60
7-99
200 66.7
10
2.04
33.0 24.8
70
9. 02
251 71 S
20
3.10
53-3 34-6
80
9-93
309 75-6
30
4-34
81.3 44-8
90
10.77
375 78-9
40
S-68
"6.7 53.9
100
"54
452 81.9
50
6.88
iSS-6 60.9
118.3
12.76
6x7 86.1
The following Sp. Gr. determinations are also given by Berkeley.
t^ 0.6 15.85 31.55 45-85 63.4 7S-6o 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 S<m-ubility and Sufersolubility Ice Curves for Rubidium Nitrate
AND Water.
(Jones, 1908.)
Gnis.RbNO>periooGms.HA X, # Prvrf Gms. RbNQi per loo Gms. H|0.
ofia Solubility Superaolubility * Jf fcS; ' Solubility SupersolubiUty
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 Rb,[H«TeO».Ci04].
Solubility in Water.
(Rosenheim and Weinbeber, xgio-xz.)
t^. o^ 20^ 30^ 40** 50^
GmS.RbtIH6TeO6.C2O4lperiOOginS.H2O 3.85 7.26 9.40 12.76 16.90
RUBIDIUM PERMANGANATE RbMn04.
One liter of aqueous solution contains 6.03 gms. RbMn04 at 7**.
(Muthm&nn and Kuntze, 1894.)
100 cc. sat. aq. solution contain 0.46 gm. RbMn04 at 2°, 1.06 gms. at 19*^ and
4.68 gms. at 60®. (Pattenon, 1906.)
RUBmiUM SBLENATE RbiSe04.
100 gms. HsO dissolve 158.9 gms. Rb|Se04 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®. (peliini, 1909.)
Results for RbHSe04 + RbHTe04. Results for RbHS04 + RbHTeS04.
Gms. per loop cc. Sat. Sol. Mol. % Selenate Gms. per loop cc. Sat. Sol. Mol. % Sulfate
RbHSeO«. RbHTeO*. in Solid Phase. 'RbHSOT " RbHTeO;. in Solid Phase.
76.46 39.51 51.55 26.675 38.403 4791
95-82 3530 52.22 32.117 31-58 5033
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 RbiSiFe.
100 gms. HiO dissolve 0.16 gm. RbiSiFc at 20^ and 1.36 gms. at I00^
(Stolba. 1867.)
RUBIDIUM SIUCGTUNGSTATE RbBSiW,2042.
100 gms. H2O dissolve 0.65 gm. RbgSiWuOis at 20^, and 5.1 gms. at 100*.
iGodeSroy, 1876.)
587
BUBmiUM SULFATE
RUBIDIUM SULFATE RbsSOi. Solubility in Water.
Solubility in Water.
(Etard, 1894; Berkel^, 1904O
Mola.
Rb3SO«
per Liter.
Gms. RbaS04 per 100 Cms.
Watuc Solution.
O
10
20
40
SO
I
I
I
I
I
2
27
46
64
79
92
04
36
42
48
S3
58
63
4
6
2
S
5
I
27 -3
29.9
32-5
34-9
36.9
38-7
60
70
80
90
100
102.4
Mols.
RbsS04
per liter.
Gms. RbtSOi per too Gma.
2
2
2
2
2
25
34
.42
49
50
Water.
Solution.
67
•4
40.3
71
•4
41.7
75
.0
42.9
78
•7
44.0
81
.8
4SO
83
.6
4S-2
The following Sp. Gr. determinations are also given by Berkeley.
74.7s 89.45 102. 4*
1.4480 1.4649 1-4753
t*. 0.5 15.80 31.6 44.2 57-90
Sp.Gr.Sat.Sol. z.2740 1.3287 '1.3704 1.3998 1.4232
• b.pt.
100 cc. sat. solution in absolute HsS04 contain 58.81 gms. RbtS04.
(Bergios, 1910.)
Solubility of Rubidium Double Sulfates in Water at 25^
(Locke, 1902.)
Per ICO cc. H2O.
Farmula.
Rb,Cd(S04),.6H,0
Rb,Co(S04)a.6H,0
Rb4Cu(S04),.6HaO
RbJ!'erSOJ,.6HaO
y ^
Gms. Mols.
Anh. Salt. Salt.
76. 7 o. 1615
9.28 0.022
10.28 0.0241
24.28 0.0579
Formula.
RbJ^n(S04),.6H,0
RbJ^g(SO0,.6H,O
RbJNi(S04),.6H,0
RbaZn(S04),.6H,0
Per too cc. giO.
Gms. Mols.
Anh. Salt. Salt.
35.7 0.0857
20.2 O.052Z
5.98 0.0142
10.10 0.023d
RUBIDIUM Dihydroxy TARTARIC ACID RbiC4H408.3HsO.
100 gms. HfO dissolve 6.M gms. RbiC4H408.3H20 at o^. (Fenton. 1898.)
On account of the unstable character of the compound, only i hour was allowed
for saturation of the solution.
RUTHENIUM SALTS
Solubilities in Water.
(Howe, 1894.)
Salt.
Ruthenium Potassium Nitrosochloride
Formula.
K2RUCUNO
«
«
u
it
u
il
n
Ammonium Nitrosochloride
ti t(
Rubidium Nitrosochloride
" " (hydrated) Rb,RuCl5N0.2HsD
Caesium Nitrosochloride CsiRuCUNO
(NH4)2RuCUNO
RbjRuCUNO
u
(t
(hydrated) Cs2RuCl6.NO. 2HsO
Gms. Salt
t*. per 100 Gmai
25 12
60 80
25
60
25
60
25
25
60
25
S
22
O.S7
2.13
"43
0.20
0.56
105.8
SACCHARIN (i, Benzosulfonazole, 2(1), one) C«H4<^'>NH-
100 parts HiO dissolve 0.4 part at 25^ and 4.17 parts at loo^
100 parts alcohol dissolve 4 parts at 25**.
100 gms. trichlorethylene aissolve 0.012 gm. saccharin at i^.
(Wei
(U. S. P. vm.)
ester and Bruins, 19x4^
SACCHABIN 588
Distribution of Sacchasin at 25** Between:
Water ♦ and Ether.
(Marden, 19x4.)
Gms. Saccharin per:
Diat. Coef.
0.267
0.235
0.245
Water f and Amyl Acetate.
(Marden, 19x4.)
Gms. Saccharin per:
xoo cc. H|0
Layer.
0.0290
0.0458
0.0719
so cc. Ether
Layer.
0.0438
0.0829
0.1245
X05 cc Aq. so cc Amyl
Layer. Acetate Layer.
0.0045 0.0700
0.0065 0.0957
O.OII4 0.1724
Dist-Coef.
0.0306
0.0322
0.0315
* Slightly acidified with HG. f Containing 5 cc. cone HCl per 100 cc.
The amount of saccharin entering the ethereal layer is increased by addition
of HCl to the aqueous laver. With 5 cc. cone. HCl per 100 cc. HsO, the distribu-
tion coefficient is reduced to 0.0624.
SALICIN C4H4(CH,.OH)O.C«HnOB.
Solubility in Several Solvents.
Solvent. r. ^°"'^vJSt.^°*** Authority.
Water 15 3.52 (Greenish and Smith, 1903.)
Water 25 4.16 <Dou, 1907.)
90% Alcohol 15 1.5 (Greenish and Smith, X903.)
90% Alcohol 15 2 (Squire and Caines, X905.)
Trichlor Ethylene 15 0.013 (Wester and Bmins, 1914O
SALICYLAMIDB 0H.C<H4C0NH,.
Distribution Between Water and Olive Oil.
(Meyer, zgoi.)
Gms. OHCeHiCONHt per xoo cc
r. 4 -* % Dist. C:oc£.
^0 Layer. Oil Layer.
3 0.056 0.126 2.25
36 0.075 0.107 1.40
SALICYLIC ACID C<H4.0H.C00H 1:2.
Solubility in Water.
(Average curve from the closely screeing determinations of Walker and Wood, 1898: at 96.4*, Philip,
Z905; at 2S*, Paul, 1894; at 20 , Hoitaema, zSoSa; Hoffman and Langbeck, 1905. For determinations
not m good agreement with the following, see Akzejew, z886; Bouigoin, 1878; Ost., 1878.)
Gms. Gms. Gms.
#• ~ CAOH.C(X)H *• (VH4.0H.C(X)H *. CA.OH.(XX)H
^- per *^' per * * per
Liter Solution. Liter Solution. Liter Solution.
O 0.8 25 2.2 60 8.2
10 1.2 30 2.7 70 13.2
20 1.8 40 3.7 80 20.5
SO 54
Solubility of Salicylic Acid in Water.
(Savorro, 1914.)
Gms. Gms. Gms.
*. C6H«.0H.C(X)H *. C.H4.OH.COOH *• C|H|.OH.COOH
^' per 1000 Gms. * per zooo Gms. * per 1000 Gms.
Sat. Sol. Sat. Sol. Sat. Sol.
o 1.24 35 3.51 70 13.70
5 I- 29 40 4.16 75 17- 55
10 1.35 45 4.89 80 22.08
15 1.84 50 6.38 85 27.92
20 2 55 7.44 90 37-35
25 2.48 60 9 95 50.48
30 2.98 6s 10.94 100 75-07
589
SALICYLIC ACm
SOLUBILITT OF SALIOTLIC ACID (LiQUID) IN WaTBR.
I>etermuiation8 by Synthetic Method. See Note, p. i6. The original data
in each case were plotted and the following figures read from the curves.
(Flaachner and Rankin, xgio.)
r.
60
70
80 12
90 19
95 crit. temp.
(Alezejew.)
Gms. CAOHCOOH per
xoo Gms.
t * ■%
Aqueous SalicyUc Add
Layer.
7
8
Layer.
68
64
58
49
«•.
60
70
80
8S
Gms. CiHtOHCOOH per
zoo Cms.
Aqueous
Layer.
45
6.5
10
IS
3-
87 ait. temp. 30
Salicylic Acid
I^yer.
68
62.5
54
46
D^ta for the melting-point curve of mixtures of solid salicylic add and water
are also given by Flaschner and Rankin.
Solubility of Salicylic Acid in Aqueous Salt Solutions at 25" and
AT 35 . (Hoffman and Langbeck, 1905.)
KCl
a
u
«
KNOt
ii
U
it
NaCl
U
t€
it
Normality
of Salt
Solution.
0.020
O.IOO
0.492
1.004
0.020
O.IOO
0.504
1.004
0.020
O.IOO
0.497
0.988
Gms.
Salt per
Liter.
1.49
7.46
36.73
74.92
2.02
10.12
51. 10
101.60
1. 19
5 -95
29.50
58.80
QH4OH.COOH Dissolved at 35". CAOH.COOH Dissolved at 35*.
.per
Gms.
Gms
1000
Sat. Sol.
2.24
2.25
2.02
1.89
2.25
2.30
2.38
2.39
2.23
2.22
2
1.72
Gm. Mol.
Per cent.
2. 9216. 10'
2.9377 "
2.6321
2. 4759
3 9351
3.0103
3.1061
3 1249
2.9110
2.9027
2.6128
2 . 2487
n
ti
tt
tt
tc
(I
tt
tt
tt
tt
Gms. per
zooo Gms.
Sat. Sol.
3-23
3.23
3.01
2.68
3.25
3 32
3.38
3.36
3.22
3.20
2.85
2.43
Gm. Mol.
Per cent.
4. 2206. 10'
4.2203 "
3.9268
3-5003
4.2499
4.3334
4.4123
4.3848
4.2062
4.1806
3-7171
3 • 1596
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
Solubility of Salicylic Aero in Aqueous Salt Solutions at 25*.
(Philip, Z905; Philip and (jamer, 1909.)
In Aq. Sodium
Acetate.
Gms. per Liter.
, • : ,
CHiCOONa. CAOHCOOH.
In Aq. Sodium
Formate.
Gms. per Liter.
1. 01
2.48
5 03
10.07
3.60
S-93
9.56
16.81
HC(X)Na.
0.81
1.63
4.06
8.14
CAOHCOOH.
3 40
4.42
7. II
10.44
In Aq. Sodium
Succinate.
Gms. per Liter.
In Aq. Potassium
Formate.
In Aq. Sodium Monochlor
Acetate.
Gms. per Liter.
CHtQCOONa. CAOHCOOH.
1.38 2.83
3-43 3-58
6.84 4.64
13.71 6.17
In Aq. Sodium Butyrate
at 26.4^
C|H«(C00Na)^ CAOHCOOH.
1. 18 2.97
2.93 4.34
S-8S 6.56
11.75 10.82
(jins. per Liter.
HC(X)K.
O
1.03
2.56
S.I2
Gms. per Liter.
CAOHCOoi? CACOONa. CaH«QHCOoS
2.265
3.38
4.93
7.13
I
2
4
S
3-3
45
6.8s
8.1
One liter of i normal aqueous sodium salicylate solution dissolves 4.97 gms.
salicylic add at 25^ (Sidgwick, x9i(v)
8AUCTUC ACID
590
Solubility op Salicylic Acid in Aqueous Solutions of Sodium
Salicylate at 20. i^
(Hoitaema. 1898a.)
Gm. Mote, per Liter.
QH«OH-
COOH.
0.0132
O.OII2
0.0124
0.0143
0.0164
0.0203
0.062
0.09s
0.09Z
0.086
0.081
0.048
0.021
o.
C«H«OH-
COONa.
o
0.017
0.113
0.226
0.344
0.500
1.70
3.IZ
2.19
4.23
4.18
4.12
4. IS
Sp. Gr. of
Solutions.
Z.002
1.003
Z.009
1. 016
Z.024
1.034
Z.I12
1.137
1. 144
1. 215
1.263
1.259
1.258
1.257
Gms. per Liter.
A
C|EI«0H-
COOH.
1.823
1.55
1. 71
1.97
2.26
2.80
8.56
13. II
12.56
11.88
IZ.19
6.63
2.90
o
CiHiOH-
COONa.
o
2.705
17.98
35.96
54.74
79 56
270.5
335-7
348.4
542.6
673
665.1
665.5
660.3
Solid Phase.
CiH^HCOOH
41
M
fl
f(
( CA0HC00H.C,Hd0HC00Na
1 +QH4OHCOOH
CsHK)HCOOH.CA0HCOONa
If
( QH^HCOOH-CAOHCOONa
( +CAOHCOONa
CAOHCOONa
14
Solubility op Salicylic Acm in Aqueous Solutions of Acids at 25*
(Kendall, 191 x.)
Acid.
Water alone
Acetic Acid
((
K
it
Fonnic Acid
u
ti
It
tt
tt
«
Gms. per Liter.
■ A
Add.
Add.
Gms. per Liter.
A — -—
C|H«0H
COOH.
o 2 . 257 Formic Acid
37.52 CHiCOOH 2.335
75.05
Add.
HCOOH
It
u
44
(f
150.10
300.20 "
2.38 HCOOH
4.59
11.05
21.17
28.76
57.53
115.07
(I
II
II
M
II
M
if
If
ff
ff
2 . 409 Hydrochloric Acid
2.549
2.850
2. 114
2.035
2 . 1 14 Malonic Acid
2.035
2.049
2.066 Methyl Picric Add
2. 121
Ha
ff
<f
230.15
460.30
0.653
X.302
4.558
9. 117
18.235
3.253 CH,(COOH),
10.49
20.84
3.28 CtHANi
II
II
II
41
II
II
CAOH-
OOOH.
2.370
2.90Z
1. 781
X.710
1.677
1.649
1. 551
2.051
1.944
1.880
2. IIS
Solubility op Salicylic Acid in Aqueous Solutions of 0 Nitrobbncoic
Acid at 25* and Vice Versa.
(Kendall, 1911.)
Gms. per Liter.
H*^
o
2.615
7.202
7.283
*CiHr
OHCOOH.
2.257
1.974
1.887
1.885
SoUd Phase.
Salicylic Add
Gms. per Liter.
■A
II
+Nltrobenioic
o C.H4.NO1.-
COOH.
7.188
7.213
7 .233
o CJL.OH.-
COOH.
2.243
1.873
1.294
Solid Phase.
0 Nitxobennic Add
Solubility op Salicylic Acid in Aqueous Alcohol at 25*.
(Sddell, 1908, X909, 19x0.)
Wt. Per cent
CAOHin
Solvent.
10
20
30
40
SO
in Sat. SoL
0.984
0.970
0.959
0.951
0.94s
Gms.
CAOHCOOH
per xoo Gms.
Sat. Sol.
0.38
0.80
2.20
5.90
12.20
Wt. Per cent
OILOHin
Solvent.
<iKofSat.SoL
Gm.<i.
CiHdOHCOOH
per xoo Gms.
Sat. Sol.
60
0.943
18.30
70
0.941
24
80
0.937
28.30
90
0.930
31-40
100
0.919
33.20
591
SALICYLIC ACm
S(X.UBiLiTY OF Salicylic Acid in Aqueous Solutions of Ethyl Alcohol.
IsoBUTYL Alcohol, Dextrose, Cane Sugar, and of Levulosb at 25*^
AND AT 35*
(Hofimann and Langbeck, zgosO
Cone, of Solvent.
CA0H.C00H DiflBolved
at 25*.
Aq. Solvent.
CJtUPE
it
tt
It
It
tt
CAOH (iso)
«
tt
QHtfO*
tt
tt
tt
CuHaOii
tt
it
tt
CHuO,
tt
tt
Normal-
ity.
0.0249
0.0560
o. 1747
0.2399
1.03
1.638
0.020
0.051
O.IOO
0.521
0.02
O.IO
0.50
I
0.02
O.IO
0.50
1. 10
0.02
0.06
0.25
Gms. per
Liter.
1. 146
2.578
8.04
11.05
47.4
75.44
1.496
3.74
7.48
38.60
3.6
18
89.6
180
6.88
34-97
172
376.3
3.6
10.8
45
Gm. Mol.
Per cent.
2.8966.10'
2.9150 "
2.9901 "
3.5279
3 9253
2.909
2.955
3.033
3.718
2.886
2.898
2.954
3.015
2.902
2.964
3.239
3.633
2.888
2.895
2.944
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
tt
Gms. per
100 Gms.
Sat. Sol.
0.222
0.223
0.229
• • •
0.270
0.300
0.223
0.226
0.232
0.285
0.221
0.222
0.226
0.231
0.221
0.227
0.248
0.278
0.221
0.221
0.225
C«jH«0H.C00H Dinolved
Gm. Mol.
Percent.
Gms. per
zoo Gms
Sat. SoL
4. 2044. 10"* 0.322
4.2348
4.229
4.289
4-435
5.624
4.184
4.202
4.263
4-360
4.206
4.287
4.697
5.236
tt
tt
4.4341
5.2816 "
tt
tt
tt
It
ft
tt
ft
It
tt
tt
tt
tt
0.324
• • •
0.339
0.404
• • •
0.324
0.329
0.339
0.431
0.321
0.322
0.326
0.334
0.322
0.328
0.360
0.401
Solubility of Salicylic Acid in Alcohols, in Ether and in Acetone.
(Timofeiew, 1891; at Z5^ Bourgoin, 1878; at 23*. Walker and Wood, 1898.) .
Gms. CiH^HCOOH
Gms. CAOHCOOH
Solvent.
f.
per IOC
) Gms.
Solvent.
f.
per IOC
> Gms.
Solvent.
Solution.'
Solvent.
Solution.'
CHsOH
- 3
40.67
28.91
C^rOKin)
- 3
26.12
20.71
CHaOH
+21
62.48
38.46
C^iORin) +21
37
.69
27.36
CAOH
- 3
36.12
26.29
(CH,),0
15
50
47
33-55
CjHsOH
+15
49.63
33.17
(CH,)/)
17
•
1 •
23.4*
CjHjOH
21
53-53
34.87
(CH,),CO
23
• 1
» •
31.3*
CiHjOH 90%
15
42.09
29.62
* Gms. per zoo cc
'. sat. sol. instead of per zoo jmu
1. sat. sol
»
100 gms. sat. solution in methyl alcohol contain 39.87 gms. salicylic acid at 15^
(Savocro, 1914.)
Solubility of Salicylic Acid in Mixtures of Acetone and Benzene at 25^
(Harden and Dover, 1917.)
Gms. per 100 Gms. Mixed Solvent. Gms. per 100 Gms. Mixed Solvent. Gms. per 100 Gtas. Mixed Solvent
^^i^^^^^^^t^^^^^mmm^^^^^^^^m^m^imm^mamm^^^am^^ ^^mmm^am^a^mmtmt^m^a^^m^Ka^^^^^^^^^^^^^m^^^^^. .^^^mam^^m^^mma^mm^^^^^i^^^^i^^^^^^^^^^^^^^^^
Acetone.
60
Acetone.
100
90
80
70
Salicylic Add.
55
51. 1
46.4
42.3
Salicylic Acid. Acetone.
36.7 20
50 31 10
40 25.3 O
3c 20
Salicylic Add.
15
7.1
0.92
II. 7
Cms. CA-
OHCOOH
per xoo Cms.
CA.
0.460
34.6
Gms. CHr
OHCOOH
per zoo Gms.
CA.
1. 261
18
18.2
25
0.579
0.78
36.6
49-4
I 430
2.380
25
18
30.5
0.991
64.2
4.40
18
SAUGYUC ACID 592
Solubility of Salicylic Acm in Benzene.
(Walker and Wood, 1898.) (von Euler and Ldwenhanm, 1916.)
Solvent. OHCOSa
per 100 cc.
Sat. SoL
CflHe 0.525
CcH« 0.762
o.snCHjClCOOHinCeHa 1.698
o. sn CftHjOH in CcH« o. 746
Solubility of Salicylic Acm in Mixtures of Benzene and Ethyl
Acetate at 25®.
(Maiden and Dover* 19x7.)
Gms. per 100 (jms. Mixed Solvent. Gms. per 100 Gms. Mixed Solvent. Gms. per 100 Gms. Mixed Solvent.
£thyl Acetate. Salicylic Acid. £thyl 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 Ra,rhniann, 19x3.)
Qoii»m» Gms. CaHiOHCOOH Q«i««f Gms. C1H4OHCOOH
Solvent. per 100 cc. Sat. Sol. Solvent. per xoo cc. Sat. Sol.
Chloroform 2 . 168 Tetrachlor Ethylene i . 105
Carbon Tetrachloride 0.4143 Tetrachlor Ethane 2.085
TricUor Ethylene i-5i9 Pentachlor Ethane 1.064
100 g:m8. dichlor ethylene dissolve 0.757 R^i- salicylic acid at 15®. ) (Wester and
100 gms. trichlor ethylene dissolve 0.28 g:m. salicylic acid at 15 . ) Brains. X9X4.)
SoLUBn^iTY OF Salicylic Acid in Oils (Temp, not stated).
(Engfeldt, 19x3.)
Gms. (jms.
Oil of- QHiOHCpOH Qji f. CJEW)HCOOH
""^'- per xoo Gms. "" ^*- per xoo Gms.
Sat. Sol. Sat. Sol.
Phocae (Dog Fish Oil) 1.70 Sesami 2.61
Jecoris AseUi (Cod Liver Oil) i . 86 Cannabis 3
Arachidis (Peanut Oil) 1.88 Lini (Linseed Oil) 3.04
Amygdalarmn 2.08 Juglandis (Walnut Oil) 3.15
Olivae (Olive Oil) 2 . 14 Gossypii (Cottonseed Oil) 3 . 23
Rapae (Rape Seed Oil) 2. 17 Ricini (Castor Oil) 12.98
Papaveris (Poppy Se^ Oil) 2. 22 Paraffiniam Liquid o
The ratio of^ the solubilities of salicylic acid in olive oil and in water (cone,
in oil -7- cone, in HxO) at 25^ is given as 11.8 by Boeseken and Waterman (1911,
1912). This corresponds to 2.6 gms. acid per 100 gms. olive oil.
Distribution of Salicylic Acm Between:
Water and Benzene. (Hendrixon, X897.) Water and Chloroform. (Hendrizon, 1897.)
Results at lo*. Results at 40®. Results at lo*. Results at 40*.
Gms. Acid xoo cc. Gms. Add per xoo cc. Gms. Add per xoo cc. Gms. Add per xoo cc.
BiO Layer. CA Layer. HaO Layer C«H, Layer.' tiaO Layer. CHCli Layer. HtO Layer. CHCU Layer.
1 0.0264 0.0391 0.0260 0.0400 0.0293 0.0442 0.0335 0.0475
0.0377 0.0655 0.0719 0.1649 0.0457 0.0946 0.0819 0.1775
0.1200 0.4159 0.1220 0.3539 O.II72 0.5640 0.1589 0.5297
0.1292 0.4713 0.1563 0.5016 0.1229 0.6196 0.2687 1.3887
0.2014 0.7625 0.1236 0.6269 0.3053 1.7570
Similar data for the distribution between water and benzene at 18^ are given
by Nemst (1891).
993
SALICYLIC ACID
Acetyl SALICYLIC ACID (Aspirin) CH,COO.C«H4.COOH, 1.2.
Solubility and Melting-Point Curves for Mixtures of Acetyl Salicylic
Acm AND Water, Determined by the Synthetic Method.
(Flaschner and Rankin, 1909.)
Solubility Curve (Liquid Add+HiO). M.-pt. Curve (Solid Acid +H^).
f.
Gma. CH(COO.CA-COOH per zoo Oma.
f.
H|0 Rkh Layer. Acid Rkh Layer.
4«o • • .
6
10
14
17s
ao
89 crit. temp. 35
SALOL (Phenylsalicylate) C«H4.0H.C00C«Hs, 1.2.
Solubility of Salol in Aqueous Alcohol at 25*.
Wt. Per cemt
25
SO
70
80
8s
87. 5
74
67
60
5S
so
82.4
90.4
92.4
93-6
99
109.4
131
Gibs. CHiCX)0C«Hr
COOH per xoo Gias.
Mtzture.
4.8
zo
20
60
80
89. S
100
^
IPHin
vent,
o
20
40
SO
60
Sat. Sol.
0.999
0.967
0.934
0.914
0.89s
Gma. Salol
per 100 Gms.
Sat. Sol.
0.015
0.020
0.22
0.76
2.10
Wt. Per cent
dH»0Hin
Solvent.
70
80
90
92.3
100
(Sddell, 1909, i9xa)
Gma. Said
per xoo Oma.
Sat. Sol.
4.40
7.70
14
17.70
3S
d^of
Sat. Sol.
0.877
0.863
0.865
0.868
0.898
Solubility of Salol in Several Solvents.
Solvent.
f.
dSat.
Sol.
Acetone
Benzene
30-31
30-31 1. 148
Amyl Acetate 30-3 1 i : 136
Aniline 30-31
Gma. Salol
per xoo Gma.
Sat. Sol.
90.99
88.57
85.29
Sdvent.
2S
Amyl Alcohol
Acetic Acid (99.5%) 21.5
Xylene 32.5
very soluble Toluene 25
100 g:m8. pyridine dissolve 381 ^s. salol at 20^-25* (Dehn, 19 17). The solu-
tion in aqueous 50 per cent pyridine separates into two layers.
Solidification Temperatures (Solubility, see footnote, p. i) for Mixtures of:
(SddeU, X907.)
J Q.^ Gms. Salol
*•• 't^** per 100 Gms.
^*- Sat. Sol.
0.869 20.44
I. 143 63.24
87.14+
I. 128 83.62
Salol and Thjrmol. (BeUucd, xgxa.)
Gms. Salol 4.0 ^t Gms. Said
per 100 Gma.
Solidif. P«rJ.<»Gms.
42
34
26
x8
13 Eutec.
17. S
Mixture.
100
90
80
70
66
60
fof
SoUdif.
23
29
34. S
40
46
51
Mixture.
SO
40
30
20
10
O
Salol and Urethan.
Gms. Salol
per zoo Gms.
Mixture.
100
fol
Solidif.
(Bdlucd, xgia, 19x3.)
Gms. Salol
per 100 Gms.
Mixture.
fof
SoUdif.
42
36.5 90
29 Eutec. 86
31 80
30 70
i4 60
36.5
39
41. S
44
47
48.5
50
40
30
20
10
o
((Bellucd,
The Eutec. for salol + camphor is at +6^ and contains 56% salol.
TheEutecfor salol+inonobromcamphor]sat2i^and contains 6o%salol. (19x2. xj.)
Solidification temperatures for Salol + Sulfonal and for Salol + fi Naphthol
are given by Bianchini (19 14).
8ANT0NIN CiiHisOt.
Solubility in Several Solvents.
Solvent.
Water
Alcohol (90%)
Trichlor Ethylene
Pyridine
Aq. 50% Pyridine
F.-pt. data for mixtures of stereoisomeric santonin salts are given by Malvino
and Manino (1908}.
f.
Gms. CuHi^ per
xoo Gms. dolveat.
Authority.
20-25
0.02-I-
(Dehn, X917)
IS
about 2.3
(Greenish and Smith, 1903.)
IS
2.46
(Wester and Bruins, X9X4.)
20-25
12.72
(Dehn, xgx?.)
20-25
".3S
M
SAMABIUM CHLOBIDl 594
SAMARIUM CHLOBIDl SaCl,.
100 gms. pyridine dissolve 6.38 gms. SaCli at 15^ (Mattgnoa, 1906, 1909.)
SAMARIUM GLTGOLATB Sa(CH«0,),
100 gms. H|0 dissolve 0.6373 gm. Sa(CtHiOi)i at 2&*.
(Jantach and GrIlDkxaut, 1912-13.)
SAMARIUM Double NITRATES.
Solubility in Conc. HNOi of da^ » 1.325 at I6^
(Jantach, 19x2.)
Samarium Magnesium Nitrate [Sa(N0i)6]Mgt . 24 Hs0 24 . 55
Nickel " " Ni, " 29.11
Cobalt " " Co, " 34.27
Zinc " " Zn, " 36.47
" Manganese " " Mn, " 5^.04
SAMARIUM OXALATE SasCCOOi.ioHiO.
One liter H2O dissolves 0.00054 S™- Sas(C^4)s at 25% determined by the
electrolytic conductivity method. (Rimbach and Schubert, 1909.)
Solubility of Saicarium Oxalate in Aqueous Solutions of Sulfuric Acid
AT 25^
(Wiith, Z9za.)
^ATttsS"' "^'^^SSl* Solid Phase. Narngmvof ^ ^(^^l' Solid Phase.
Aq.H,S04. Sat. Sol. Aq. H^SO,. "sat. Sol.
I O.IOI5 Sai(C^4)|.xoHi0 2.8 O.3886 SacCC^Ja-zoH^
1.44s 0.1804 " 4.32 0.7008
1.93 0.2254 " 6.175 1.072 "
SAMARIUM Dimethyl PHOSPHATE Sa,[(CH.)sP04]«.
100 gms. HsO dissolve 35.2 gms. Sas[(CHi)sP04]« at 25^ and about 10.8 gms.
at 95^- (Morgan and James, 19x4.)
SAMARIUM SX7LFATE SasCSOOi.
Solubility in Aqueous Solutions of Ammonium Sulfate at 25®.*
(Keyes and James, 19x4.)
OTW.S04.
Sa,(S04),:
Solid Phase.
(NH4),S04.
Sa^SOi),:
Solid Phase.
0.03
0.8
2.1
2
Sai(S0J,
It
32. s
46.3
0.9
I
1.1.7
I.I
2.8
" +X.1.7
77.5
1.3
" +(NH4),S04
1.9
7.4
18.8
0.8
0.8
X.X.7
11
77.3
76.8
0.3
0.6
(NHJtSO*
M
1.1.7 = Sa,(S04)i.(NH4)sS04.7H,0.
Solubility in Aqueous Solutions of Sodium Sulfate at 25**.*
(Keyes and James, X914.)
Gms. per 100 Gms. H^O. „ ...... Gms. per 100 Gms. HjO. _ ... _.
"-•-« *»«^ - Solid Phase.
sSai(S04)|.3Na«SO«.6HiO
Na,SO«.
Sa,(S04),.
SoUd Phase.
Na,S04.
Sa,(S04),.
• • •
2.05
Sa,(S0J,
10.51
0.012
O.I
2
<i
14.71
O.OIO
0.5
O.II
3Sa,(S04)s.3Na«SO«.6H^
20.02
0.012
1.9
0.03
u
23.68
0.018
6.44
0.016
u
27.40
O.OII
M
M
* The mixtures were rotated at constant temperature for 5 months.
ibo cc. anhydrous hydrazine dissolve i gm. Sas(S04)i at room temp.
(Welsh and Brodenon, 1915.)
595
SAHABIUM 8X7LFONATES
SAlfABIUM SX7LFONATB8
Solubility in Water.
Salt.
Fonnuh.
Gm. An*
M hydiuusSalt
* per xoo Gms.
H|0.
Authority.
Samarium tn Nitro-
benzene Sulfonate Sft[C«EU(NO0SQ||t.7H^ 15
Samarium Bromonitro-
benzene Sulphonate Sa[C«Hs(x)Br<4)N0^a)S0j|.ioH^ 25
SCANDIUM OXALATE Sc(C^4)i.5H,0.
Solubility in Aqueous Solutions of Ammonium Oxalate and of Hydro-
chloric Acm.
50.9 (Holmbeis, 1907.)
7 . 84 (Kats and James, X913O
In Aq. Ammonia Oxalate at 25^
(Wirth, 19x4)
Cms. per xoo Gma.
Sat. Sol.
In Aq. Hydrochloric Add at 25*
and at 50®. (Mejer, X9I4-)
CA.
1.624
2.4
4.478
ScA.
0.3019
0.4012
0.7108
Solid Phase.
Sc(C^J, sEfi
If
H
+(NH4),Q04
Normalitvof
Aq. HCl.
O.I
0.5
I
2
5
GiiiB. ScsCQOJa per
xoo Cms. Sat. Sol.
At as*.
0.0299
0.0650
0.1020
O.1716
0.4170
At so*.
0.0420
0.0870
0.1435
0.2556
0.6533
Solubility in Aqueous Solutions of Sulfuric Acid.
Results at 25®. (Wirth, 19x4.)
Nonnality_of ^^,^^^^
Sat. Sol.
Aq. H|Sb«.
I
2.1
2.43
3.57
4.86
O.I 148
0.2S73
0.2904
0.4204
0.5834
Solid Phase.
Sc(CiOJ^sHiO
u
M
Results at 25** and at 50**. (M^yer, 19x4.)
xnality ol
.1^4.
Normality of
Aq.
Cms. SciC&OJi per xoo C^ns.
Sat. Sol.
u
O.I
0.5
I
2
S
At 25*.
0.0385
0.0997
0.1663
0.3176
0.7761
At 50*.
0.0562
O.I481
0.2493
0.4429
I. 1280
Solvent.
Cms. SciCSOJi
per 100 Gros.
Sat. Sol.
Solid Phase.
100 gms. sat. solution of scandium oxalate in 2.43 n HtSOi + 0.5 n oxalic
acid contain 0.0284 gm. ScsOs at 25**. (Wirth, 19x4.)
SCANDIUM SX7LFATE ScsCSOOlsHsO.
Solubility in Water and in Aqueous Sulfuric Acid at 25°.
Gms. SciCSOJi
Solvent. per xoo Qma.
Sat. SoL
Water 28.52 Sc^sodB.sW> 4.86nHiS04 8.363
o.5fiH«S04 29.29 " 9.73fiHtS04 1.315
I nHjS04 1987 " 22.35nH,S04 0.484
Scandium sulfuric acid double sulfate, Scs(S04)i.3HtS04. 100 gms. sat. sol. in
cone. HsS04 of dt = 1.6 contain 0.8616 gm. of the double salt. (Wirth, 19x4.)
8EBACIC ACm (CHs)s(COOH)s.
100 gms. 95% formic acid dissolve 1.05 gm. sebadc add at 19**. (Aschan, 19x3.)
Distribution op Sebacic Acid between Water and Ether at 25^
(Chandler, 1908.)
(Wirth, 1914.)
Solid Phase.
Sc(S04),.5Hi0
SGk(S04)|.3H/)
Mol. Concentration of Sebacic Add in:
Ratio.
0.0213
Aq. Layer. Ether Layer.
0.00062 0.0291
0.00058 0.0272
0.0213
0.00047 0.0213
0.0221
0.00036 0.0155
0.0232
8ILSNIUM 59^
8ILSNIUM Se.
Solubility in Carbon Disulfidb.
(Marc, Z906.)
100 cc. CSi dissolve 0.065 gm. amorphous Se at room temperature. Se which
is heat^ to 180° for 6-7 hours is insoluble in CSs. Se crystallized from the
melt at 200^ is insoluble in CSs. Se heated once quickly to 140^ is very slightly
soluble in CSt.
100 cc. CSs dissolve at the boiling-point 3-3.4 mgs. Se which has been heated to
140* for I hr.
100 cc. CSs dissolve at the boiling-point 2 mgs. Se which has been heated to
195^ for 2 days. (Ifaic, 1907.)
.100 gms. methylene iodide (CHsIs) dissolve 1.3 gms. Se at I2^ (ReCcefs, 1893.)
Solubility op Mix Crystals op Sblbnium and Sulfur in Carbon Disulfidb
AT 25'. (Ringer, xgoj.)
Mols. per 100 Mob. Solution. MoJ- /«F
Cent Se in
CrysUls.
O
3-54
3.81
8.69
16.4^
14.2*
29.35*
* Mix oystalfl homogeneous in all except these sdutions.
t « Solubility of hexagonal selenium. | « Solubility of amorphous aelenium.
Fusion-point curves for mixtures of selenium and other metals are given by
Pelabon (1909). Results for Se -f- Te are given by Pellini and Vio (1906).
Diohenyl SELENIUM BBOIODB (QHOsSeBrt.
^"RSCIFROCAL SOLUBILITY OP DiPHENYL SeLBNIUM BrOMIDB AND DlFHBNYL
Tellurium Bromide in Water at 25^.
(Pellim, 1906a.)
Gn». per loop cc. Sat. Sol M<J. % (C|H,)r Gna. per locp cc. Sat. Sol. Mol. % (QWs-
(CA).TeBr.. (CHOt-SeBr.. ^ll^^ tCA).TeBr.. ' (CA).ScBr; ^ ^^ASiS?^
18.614 o o 10.224 14.608 4489
17.400 1.448 4.91 7. 544 19.876 51.18
16.152 4.173 10.51 6.780 18.984 94.25
15.030 6.210 18.21 3.184 17.392 95-83
13-320 8.148 24.98 o 18.984 100
11.940 11.420 34.94
SELENIC ACm HsSe04
Solubility in Water, Determined by Freezing-point Method.
(Kremann and Hofmeier, 1908.)
CS,.
Se.
S.
43.x
0
56.9
45.1
0.93
53.97
44.98
1.03
53.99
47.84
2.07
50 -59
49.54
2.19
48.27
47.62
2.16
50.22
46.12
1.485
52.39
Mob. per 100 Mols. Solution.
MoLPer
OntSein
Cryttah.
55 67
68.38
58.7
CS,.
58.24
64.66
81. IZ
Se.
2.35
1.58
2.4
s. •
39-41
33.76 .
16.49
88.41
91.38
2.17
1.68
9.42
6.94
61.5
99 51
0.49
0
loot
99.14
0.86
0
zoot
C^ms. HtSeOf
Qna,Tl^StOi
f.
per xoo Gma.
Sat. Sol.
SoUd Phase.
t* . per xoo Gms.
Sat. Sol.
Solid Phase.
0
0
Ice
-55 71.5
BSeOi-ABfi
— 10
21
fi
—65 Eutec 74
" +H«Sea,.^0
— 20
30
M
-50 75.5
H.SA.HdO
-30
36
U
-20 79
u
-40
40
M
0 81
M
-50
42.5
«
+20 85
M
-60
45
M
26 m. pt 88
M
-80
48
M
20 91
M
—95 Eutec.
50
" +HiSe04.4HiO
16 Eutec 91. 5
« +HiSeO,
-80
52
B^SeO«.4H«0
30 93
BiSeOi
-70
54
M
40 94.5
M
-60
^ S8
M
50 96.5
«
—51 m.
Pt.
67
M
60 zoo
u
597 SILENIOUS ACID
SEUBNIOUS ACID HsSeO,.
Solubility in Water.
(Etard, 1894.)
^ Gms. HgSeOi per ^
Cms. H|Se0| per
t*
Gnu
. HiSeQiper
* • xoo Gms. SoluUon. * *
xoo Gms. Solution.
* .
xooGms.Soludon.
— 10 42.2 2$
67
60
79-3
0 47-4 30
70.2
70
79.3
+10 S5 40
77S
80
79.3
20 62.5 so
79.2
ium Dioxide) SeO|.
90
79-4
SEUBNIOUS AMUYDRIDE (Seleni
Solubility in
Several Solvents.
(de Coninck, 1906.)
Solvent.
to Gms. SeOi per
100 ccSolvent.
Water
"•3-iS
38. S
Ethyl Alcohol (93%)
14. 1
10.2
Methyl Alcohol
II. 8
6.66
Acetone
IS -3
4. 35
Acetic Acid (Glacial)
12.9
I. II
8IUCA SiOi.
Solubility in Water and in Aqueous S(x.utions of Acids.
(Lenher and Merrill, xgx?.)
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
HCl 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 HFl -f- HtSOi. The difference was considered to show "the amount
of silica which hiad changed from an unfilterable to a filterable state of division."
Results for Aq. HCl: Results for Aq. HtSOi:
At 25^ At 90*. At 90*.
Per cent Gm. SiOi per Per cent Gm. SiOb per
HQ. 50 cc. Sol. HQ. 50 cc. Sol.
o 0.0080 o 0.0213
3 0.00665 2 0.0198
6.3 0.00465 3 0.0186
II. I 0.00245 5.4 0.0152
18.9 0.0008 7,6 O.OII5
25.1 0.0006 10 0.0091
34.6 0.0003 13.6 0.0056
18.6 0.0029
At 90°, a slow current of COi through the solutions did not affect the results.
Ignited silica reaches eauilibrium very slowly as compared with silica gel. The
true solubility of ignited silica is probably the same as that of gelatinous silica.
Solubility op Silica in Melted Calcium Chloride.
(Amdt and Lowenstein, 1909.)
Percent
Gm. SiOi pe
50 cc Sol.
HtSO«.
3-9
0.02II
7-3
0.0186
156
O.OII2
254
0.0058
36
0.0034
46.9
0.0013
55-6
0.0005
71
0.0004
f.
Gnu. SiOk
per 100 Gms.
Sit. Sohitioo.
800
2-5
850
3.8
900
S-4
9SO
7.6
SILICON
Si
598
Solubility in Lead, in Zinc
AND
1 IN Silver.
(Moiaaan and Siemens, 1904-)
In Lead.
In Zinc.
In Stiver.
f.
Gm. Siper
100 Gms Lead.
f.
Gm. Siper
100 Gms. Zinc.
f.
Gm. Si per 100 Gms.
Silver.
1250
0.024
600
0.06
970
9.22 (58.02)
1330
0.070
650
o.iS
1150
14.89 (27.66)
1400
0.150
730
O.S7
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 I
to be incompletely soluble in HF. The figures in parentheses show the per- 1
centage soluble in HF in each case. I
Freezine-point data for mixtures of silicon tetraphenyl and tin tetraphenyl
are given by Pascal (1912). '
SnJCON IODIDES Si,I«, Sih.
Solubility in Carbon Disulfide.
(Friedel and Lachbuis. 1869; Friedd, 1869.)
100 gms. CSt dissolve 19 gms. Si|I« at 19".
100 gms. CSt dissolve 26 gms. Sitle at 27**.
100 gms. CS| dissolve 2.2 gms. SiU at 27^.
SIUCO TUNGSTIC ACID HsSiWisOn.
100 gms. H|0 dissolve c^i.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 CH,COOAg.
Solubility in Water.
(Nemst, 1889; Arrlienius, 1893; Goldschmidt, 1898; Nauman and Ruc^er, 190$: Raupcostiauch,
1885; Wright and Thompwon, 1884, 1885.)
f.
Gms.AgCCsHsOa)
per Liter.
t».
Gms.Afl[(CsH«Oi)
per liter.
t*.
Gms. AffCCtHsOs)
perliter.
0
7.22
25
II. 2
SO
16.4
10
8-75
30
12. 1
60
18.9
IS
9 4
40
14. r
70
21.8
20
10.4
80
25.2
Solubility of Silver Acetate in Aqueous Solutions of:
Silver Nitrate. Sodium Acetate.
Gms. Gma. CH»COOAg per Liter at; chJcSoN p°»- CHaCOOHg per Liter at;
palite?. id^'CNecnst). ig^(Airbenius). pS'Uter.* 16* (N..N.andR.). i8-6<'(A.)7*
0
10. OS
98s
0
10.05
9.9
5
8.3
7-9
5
63
6.6
10
7.0
6.6
10
4.6
4.9
IS
6.4
55
IS .
3-8
4.1
30
5-7
45
30
3-3
3 5
30
4.4
• « •
30
• • •
2.8
40 3*2 * * * 40 • • • 3 '4
599
8ILVEB ACETATE
Solubility of Silver Acbtatb in Aqueous Salt Solutions at 25^*. aaqun, 1910.)
Aq. Solution of;
Water alone
Cadmium Acetate
It
It
t(
t(
tl
It
Lead Acetate
tt
tt
tt
tt
tt
tt
tt
Gms. Salt,
per Liter.
O
5-76
11.52
57-6
115. 2
1.63
8.13
16.26
81.3
162.6
Gms.
AgOEW.
per Liter.
11.08
10.39
8.10
6.71
4-33
3.95
10.69
9-45
8.34
7.26
S-99
Cms. Salt
Gms.
Aq. Solution of: ^^^to^ AgCjHA
Potassium Acetate
(( tt
perJ
2.22 9.60
tt
tt
tt
tt
Silver Nitrate
tt tt
tt
tt
tt
tt
Sodium Acetate
tt tt
tt
tt
tt
tt
22.2
III
222
2.77
S'SS
II. 10
22.21
1.97
19.7
98. s
197
4.43
2.41
2.18
9-93
9
7 41
S.81
9.27
4.21
2.33
2.07
Solubility of Silver Acetate in Aqueous Scx^utions of Nitric Acm at 25^.
(Hill and Simmons, 1909.)
Normality of Per cent HNOb in
Aq. UNO^.
O
0.50
I
2
4.02
503
6.44
Sclent.
O
3 096
6.128
"•757
22.386
27.328
33-813
Sat. Sol.
1. 005
1.072
1. 140
1.267
1.470
1.561
1.670
Gms. A«C|HA
per Liter Sat. Sol.
II. 13
85.31
161. 9
307.4
549-3
656
792.2
Results are also given for the solubility of AgCsHiOs+AgNOi in Aq. HNOt at 25^
SoLUBiLrrY OF Silver Acetate in Aqueous Solutions of Several
Compounds at 25^ (Armstrong and Eyre, 19x3.)
Aqueous
Solution of:
Gms. Gms.
Compound AgQHA
Water
Acetaldehyde
Paraldehyde
xooo Gms.
O
II
II
33
66.4
per xooo
Gnw.
Sat.SoL
11.08
10.13
8.92
9.16
7-55
Aqueous
Sdution of:
Propyl Alcohol
it
tt
Glycerol
Glycol
Gms.
Compound
P^
xooo Gms.
IS
60
9.21
15.5
62.1
Gms.
AgQHA
per xooo
Gms.
Sat. Sol,
9.88
8.03
8.66
10.86
8.44
Isobutyl Alcohol
SILVER MonochlorACETATE CHtClCOOAf .
One liter aqueous solution contains 1 2 .97 gms. CHtClCOOAgat 1 6.9°. (Arrhenius/93.)
Solubility of Silver Mono Chlor Acetate at 16.9*
Aqueous Solutions of:
in
Silver Nitrate.
Sodium Chlor Acetate.
f
Gms.
A«NOs
per liter.
— *•■ — \
Gms.
CHjClCOOAg
per Liter.
Gms.
CHsaCOONa
per Liter.
Gms.
CHaQCOOAi
per Liter.
0.0
12.97
0.0
12.97
9.6
10.05
3.88
10. 05
17.0
7-55
7.77
8.16
IS 53
6.02
31.07
58.26
4.19
3-26
SILVER AGITATE 600
SoLUBiLiry OF Silver Monochloro Acbtatb in Nitric Acid at 25*
(Hill and SimmonSp 1909.)
Nonnaltty
Gmt-HNOb
Sat. Sol.
Gms.
of Ag.
HNOk.
per zooGms.
Solveiit.
AgCAClQ,
per Liter.
0
0
1.009s
IS 18
0.25
I
.564
1.0426
50-33
0.50
3
.096
I. 0791
91.83
I
6
.128
I . 1473
167.3
2
II
•757
I. 2716
310-8
4
22,
.277
1.4749
549- 1
S
27
.185
I 5673
659.2
SILVER Dipropyl^ ACETATE AgCtHuOs. .
100 gmsT H|0 dissolve 0.123 gin. AgCsHuOt at 11.7*, and 0.190 gm. at 72®.
(Forth, 1888.)
SILVER Methyl Ethyl ACETATE Ag.CH|.CHtCH(CHs)COO.
SILVER Diethyl ACETATE Ag[(C,H»),CH.COO].
SILVER Trimethyl ACETATE Ag(CHi)«CCOO.*
Solubility of Each in Water.
(Sedlitzky. 1887; Keppkh. 1888; Stiassny, 1891.)
*•
Gms.
per 100 Gms.
H,0.
AgCOIA.^
f.
Gms.
per xoo Gms. H|0.
Ag.C»H|0|.
A«C^uO,.
A«caiA.
A«CaiuO|.
A«CJI*0».*
0
1. 112
0.402
1. 10
50
1.602
0536
1-47
10
1. 126
0.413
I. IS
60
1.827
0.585
1-57
20
1. 182
0.432
1.22
70
2.093
0.643
1.68
30
1.280
0.458
1.22
80
2.402
• • •
1.80
40
1.420
0.494
1-37
SILVER ARSENATE Ag,As04.
One liter HsO dissolves 0.0085 S™* AgsAsOi at 20^. See Note, p. 608. (Whitlv* 2910.)
SILVER ARSENITE Ag»AsOi.
One liter HsO dissolves o.oi 1 5 gm.Ag<AsOi at 20**. See Note, p. 608. (Whitlv. 1910.)
SILVER BENZOATE CeH.COOAg.
One liter of aqueous solution contains 1.763'gms. C«HsCOOAg at 14.5^, and 2.607
gms. at 25°. (HoUeman, 1893; Noyes and Schwartz, 1898.)
Solubility of Silver Bbnzoate at 25^ in Aqueous Solutions of:
Nitric Acid (N. and S.). Chloracetic Acid (N. and S.).
Gms. Mols. per Liter. Gms. per liter. Gms. Mols. per Liter. Gms. per Liter.
/ * \ / * \ / * -\ t * -\
^^^- cooAg. ^^^* cwAg. cic<Sh. co^. cico6h. co6a«.
o 0.01144 o 2.607 o 0.01144 o 2.607
0.004435 0.01395 0.280 3195 0.00394 0.01385 0.371 3.172
0.00887 0.01698 0.559 3889 0.00787 O.O1612 0.744 3.691
0.00892 O.OI715 0.562 3.926 0.01574 0.02093 1.487 4.792
0.01774 0.02324 I. 118 5.321
0.02674 0.03071 1.686 7.031
One liter of cold alcohol dissolves 0.169 gm. C«H|COOAg; one liter of boiling
alcohol dissolves 0.465 gm. (Uebennaan, 1903.)
SILVER BORATE AgBOi.
One liter of aqueous solution contains about 9.05 gms. AgBOs at 2^^.
(Abegg and Cox, 1903.)
601 SILVEB BBOMATE
SILVER BBOMATE AgBrOi.
Solubility in Water.
t* . Gms. AgBiQi per Liter. Authority.
20 1 . 586 (Bflttger, 1903.)
24.5 1. 911 (Nqyes, 1900.)
25 1.68 (Longi, 1883.)
27 ^ • 7 ^ (Whitlv, 19x0, aee note, p. 608.)
25 1.949 (Hm.1917.)
SOLUBILITT OF SiLVER BrOICATB IN AqUBOUS AcBTIC AcID AT 25^
(HUl, 1917.)
Normality of Aq. Gms. A^BiQi per Normality of Aq. Gms. AxBiO^ per
Acetic Add. Liter. Acetic Acid. Liter.
0.0498 1-9429 0.4988 1.863
0.0997 1.9379 0-9975 I. 8013
0.1995 1.9206 1.872:^ 1. 6178
Solubility of Silver Broicatb in Aqueous Ammonia and Nitric
Acid Solutions at 25®.
(LoDgi, X883.)
Sdvent. Gms.AgBK>.per
xooo cc. Sol. xooo 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 op Silver Bromatb at 24.5^ in Aqueous
Solutions op:
Silver Nitrate (Noyes). Potassitmi Bromate (N.).
Normal ^Content. Gms. per liter. Normal Content. Gms. per liter.
A«NQt. AgBrOs. AgNOs. AgBrOt. KLBrOs. AgBrOt'. &BrO|. AgBrOft.
0.0 0.0081 0.0 1. 911 0.0 0.0081 0.0 I.9ZI
0.0085 00051 1.445 1.203 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.
Aatfaority.
(BOttger — Z. physik. Ch. 46k 60s, '03.)
(Abegg and Cox — Z. physik. Ch. 46b xxi '03.^
(BAttger — Z. physik. Ch. s6, 93^ *o6.)
(See also HoUeman — Z. physik. Ch. zat xsp, '93; Kohlrausch — Ibid, 50^ 365, '05.)
Solubility op Silver Bromide in Aqueous Ammonia Solutions.
(Loogi — Gazx. chim. ital. za, 871 '83; at 8o^ Pohl — Sitzber. Akad. Wiss. Wien, 41* S67, '60.)
Gms. AgBr at xa*' per Qms. AgBr at 80* per
Solvent. xooo cc. 1000 Gms. *«» Gms.
Solvent. Solvent. Solvent.
Ammonia Sp. Gr. 0.998=5% 0.114 0.114
Ammonia Sp. Gr. o .96 = 10% 3 .33-4 o 3 .47
Ammonia Sp. Gr. 0.986 ... ... 0.51*^ i. of
* Dried AgBr. t Fleshly pptd.
f.
Gms. AgBr per Liter.
20
0-000084
as
0.000137
100
0.00370
8ILVEB BBOMIDl
603
Sat. Sol.
Solubility of Silver Broiodb in Aqueous Ammonia Solutions.
Results at 15"*. Results at 25**. Results at 25'.
(BodUoder and Fittig, x9ox-oa.) (Wbitnor and Mdcberp 1903.)
Gms. Mols. per looo Gms. HgO. Concentration per Liter.
G. Mols. NH«. G. Atoms Agl
(Bodliader, 1893.)
Gms. Mols. per Liter.
0.9932
0.9853
0.9793
0.9720
O.96SS
NH«.
1.085
2.365
3 410
4.590
5-725
A&Bfi.
O.OOII
0.0031
0.0050
0.0074
O.OIOI
NH«.
0.1932
0.3849
0.7573
1.965
3.024
5244
A«Br.
0.00060
0.00120
0.00223
0.00692
O.OI163
0.02443
0.0764
O.II5
0.268
0.273
0.450
0.497
0.000276
0.000391
0.000941
0.00107
0.00170
0.00159
SOLUBILITT OF SiLVER BrOMIDB IN AQUEOUS SOLUTIONS OF:
Ammonia at o**.
Qany. 1899)
Grams per xoo oc. Solution.
Monomethyl Amine at 11.5^.
(Jarry.)
NHsGas.
3 07
4.88
6.69
8.29
II. 51
15 32
18.09
19-53
AcBr.
0.080
0.096
0.172
0-2I2
0-349
0557
0.722
0.741
NHsGas.
26.27
31
33
36
37
37
39
39
26
89
52
22
70
26
95
AgBr.
1.067
1.568
1.987
2.669
2.888
2.930
2.892
a. 852
w. p
er xoo c
c aonxnon
MHiCH>.
AgBr.
II .01
0.07
13
17
0.12
IS
13
0.16
17
97
0.28
32
58
0.55
35
.63
0 73
43
.11
1.27
48
44
2.89
SOLUBlLITT OF SILVER BROMIDE IN AqUEOUS SOLUTIONS OF MBTHYL
Amine and of Ethyl Amine at 25^
(BMIander and Khwrkin, 1903; Wath, 1903.)
In Methyl Amine.
Mols. per Liter.
^otalBase. A«Br. Free Base.*
1. 017 0.0025 I.OI2(B.&E.)
Jn Ethyl Amine.
Mols. per Liter.
f otal Base. AgBr. Free Base.*
• 0.483 0.00231 0.478 (B.&E.)
0.508 0.0013 0.505 (B.&E.) 0.200 0.00097 0.198
0.203 0.00049 0.202 (B.&E., W.)o. 100 0.0004750.099
€1
0.102 0.00026 0.102 (B.&E.)
0.09470.00041 ... (W.)
0.051 0.00012 0.051 (B.&E.)
0.04 0.00034 ... (W.)
0.02 0.00026 ... (W.)
0.103 0.000711
0.06572 0.000258
0.05512 0.000193
0.03942 0.000137
0.01272 0.0000867
(w.)
tt
It
a
it
* The &ee base b found by subtracting from the total base tiro mols. of base for each atom of dissolved Ag.
S(H.UBILITY OF SILVER BrOMIDE IN AqUEOUS SOLUTIONS OF MERCURIC
Nitrate at 25*.
(Morse, 1902.)
Gms. AgBr
per Liter.
6.878
1.640
1.200
Mob. HgNOr
(HNOk) per Liter.
I
O.IO
0.05
Mols. AgBr
per liter.
0.03660
0.00873
0.00639
Mols. HgNOr
Mols. AgBr
Gms. AgBr
(HNOi) per liter.
per Liter.
per Liter.
0.025
0.00459
0.863
0.0125
0.00329
0.618
O.OIOO
0.00306
0.57s
Since HNOs 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 HNO^ Both crystallized and
amorphous nlver bromide gave identical results.
6o3
SILVER BROMIDE
Solubility of Silver Bromide in Aqueous Salt Solutions.
(Mees and Piper, 19x2.)
Aqueous Solution.
Aq. I per cent Sodium Thiosulfate
" " Ammonium Thiocyanate
" " Ammonium Carbonate
" Sodium Sulfate
Thiocarbamide
t<
ti
?
(I
u
ti
Cms. AgBr
per Liter.
2.06
0.03
0.004
o.oss
1.49
Solubility of Silver BROiimE in Aqueous Salt Solutions.
(Valenta, 1894; see also Cohn, 1895.)
Salt Solution. t*.
Sodium Thio Sulphate 20
" Calc. by Cohn 20
Sodium Sulphite 25
Potassium Cyanide 25
" Calc. by Cohn 25
Potassium Sulphocyanide 25
Ammonium Sulphocyanide 20
Calcium Sulphocyanide 25
Barium Sulphocyanide 25
Aluminum Sulphocyanide 25
Thio Carbamide 25
Thio Cyanime 25
Gms. AgBr per xoo Cms. Aq. Solution of Concentration:
x: 100.
0-3S
0.50
5: xoo.
1.90
2.40
• • •
6-55
6.8s
• • •
0.21
0.08 0.35
xo: xoo.
3 SO
459
0.04
0.73
2.04
053
0-3S
4 50
1.87
0.72
X5: xoo.
4.20
6.58
so: xoo.
5.80
8.40
0.08
S-30
• • •
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(AgSiOiNa)s, instead of the more soluble tri salt, (AgSiOiNa)2NaflSsC)t.
100 cc. HsO containing 10 per cent of normal mercuric acetate, Hg(CtHiOt)s+
Aq., dissolve 0.0122 gm. AgBr at 20^.
100 gms. NaCl in cone. aq. solution dissolve 0.474 gm. 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 . (Schierhols, X890.)
Solubility of Silver Bromide in Aqueous Potassium BROMroE at 25®.
(Hellwig, X900.)
Mols. KBr per Liter 2.76 3.68 4.18 4.44 4.864
Gms. KBr per Liter 2.20 7.50 13 S© 17 -95 26.44
Solubility of Silver Bromtoe in Aqueous Solutions of Sodium Sulfttb.
Results at Room Temperature (?).
(Mees and Piper, xgxa.)
Gms. per Liter.
, •
Na«S0».
Gms. per Liter.
Results at 25*.
(Luther and Leubner, xQxaa.)
Gms. Formula Weights
per Liter.
0.08
0.17
0.30
0.59
113
2.08
AgBr.
0.000746
0.00219
0.00393
0.00448
0.00865
0.01585
Na,SQ|.
4.85
9-47
17.65
38.2
70 -75
83.7s
AgBr.
0.0329
0.05264
O.I16
0.265
0.57
0.79
SO,".
0.232
0.406
0.448
0.466
0.474
0.67s
Ag'.
0.0025
0.0023
0.0023
0.0053
0.0055
0.0084
SILVER BROIODI
604
Solubility of Silver Bromide in Aqueous Solutions of Sodium
Thiosulfatb at 35®.
(Richards and Faber, 1899.)
Gms. Cryst. Na
ThioBulfate
per Liter.
100
200
300
400
Gms. AgBr
Dissolved per Gm.
of ThiosuJphate.
0.376
0.390
0.397
0.427
Mols. A^Br
Dissolved per
Mol. of Nai^
0.496
0.515
0.524
0.564
100 cc. of 3 ff AgNOs solution dissolve 0.04 gm. AgBr at 25**. (HeDwig, 1900.)
Fusion-point data for mixtures of AgBr + AgCl and AgBr + Afi^I are given by
M6nkemeyer '(1906). Results for AgBr + NaBr are given by Sandonnini and
Scarpa (1913).
SILVER BUTTRATE CiHTCOOAg.
SILVER (l8o)BUTYRATE (CH,)sCHCOOAg.
Solubility of Each Separately in Water.
(Goldscfamidt, 1898; Arrhenlus, 1893; Raupenstrauch, 1885.)
t?
Gms. per
100 Gins.H/).
30
40
so
60
70
80
Gms.
per 100 Gms. H^.
b *
0
10
17.8
18.8
20
25
Butyrate.
0.363
0.419
0.432 (A.)
0.445 (A.)
0.484
• • •
Iso Butyxate.
0.796
0.874
• • •
• « •
0.961 (0.9986)
. . . (1.0442)
r"
Butyrate.
0.561
0.647
0.742
0.848
0.964
1. 14
Iso Butyrate.
1.060 (1.IO22)
1. 176 (R.)
^'3^3
« • ■
1.670
1.898
Solubility op Silver Butyrate in Aq. Solutions of Silver Acetate,
Silver Nitrate and of Sodium Butyrate.
In Silver Acetate at 17.8®.
G. Mols. per Liter. Grams per Liter.
CH, CsHt
COOAg. COOAg.
0.0 0.0221
0.0270 0.0139
0.0506 0.0103
CH3 C3H7
COOAg. COOAg.
0.0
451
8.45
(Arrhenius, 1893.)
In Silver Nitrate at i8.8*.
G. Mols, per liter.
A«NO,. cooig.
4.32 0.0 0.0228
2.71 0.0667 0.0078
2.01 o.ioo 0.0062
In Sodium Butyrate at 18.2'
CJ1H7
COONa.
0.0
0.0066
0.0164
0.0329
CsHt
COOAg.
0.0224
0.0199
0.0169
00131
C3H7 CjHt
COONa. COOAg.
0.0 4.363
0.73 3.881
I. 81 3.296
362 2.555
CsHt
COONa.
0.0658
01315
0.263
0493
CsHt
COOAg.
0.0091
0.0060
0.0040
0.0027
Grams per Liter.
A«N0». c§§ig.
0.0 4-445
11.33 I. 521
17.00 1.209
G. Mols. per Liter. Grams per Liter. G. Mols. per Liter. Grams per Liter
* ■■> < * > < * t « *
CgH,
COONa.
7.24
14.47
28.96
54.28
CdH,
COOAg.
-1.774
1. 170
0.780
0.526
%
6o5 8ILVEB CAPB0ATE8
SILVER CAPB0ATE8 Ag(C<HiiOi).
Solubility of Each Separately in Water.
(Keppish, 1888; Stiaasny, 1891; Kulisch, 1893; Kdnig, 1894; Altschul, 1896.)
Results in terms of gms. salt per 100 gms. H2O.
a Methyl Pentan Methyl 3 Pentan 4 Methyl Pentan
Caproate 4 Acid had 4 4 Add
)4COOAg. Cl£.CH.CH» CHa-CH, CH8(CHa)sCH(CH«)
Normal Cai
CHa(CH2)4
.(CHi^aCOOAg. .CHCHsCHjCOOAg. '.COOAg.
O 0.076 (a.) O.oySCKeppiah) 0.l68(K5nig) o.88o<Kuliah) 0.5IO(Stiaa5Dy)
10 0.085 0-089 0.162 0.858 0.528
20 o.ioo 0.107 0.163 0.849 0550
30 0.123 O.I3I 0.170 0.854 0.574
40 0.154 O.161 0.183 0.871 0.602
50 0.193 0.198 0.203 0.902 0.632
60 0.240 0.243 0.229 0.946 0.666
70 0.295 0.288 0263 I 003 0702
80 0354 ... 0.300 1073 ^0.742
90 ... ... 0347 1*^57
SILVER CARBONATE AgtCOs.
Solubility in Water.
t*. . Gms. Ag^COi per Liter. Authority.
15 0 . 03 1 (Kremers, 1852.)
25 0 . 033 (o.ocx>x2 gm. atoms Ag.) (Abegg and Cox, 1903.)
25 0 . 03 2 G^y potential measurement) (Spencer and Le Pla, 1909.)
100 0 . 50 Qoulin, 1873.)
15 0 . 85 (in H|0 sat. with CQi) (Johnson, x886.)
SILVER CHLORATE AgClO,.
icx> gms. cold water dissolve 10 gms. AgClOs (Vauquelin); 20 gms. AgClOi
(Wachter).
SILVER CHLORIDE AgCl.
Solubility in Water.
(A laige number of determinatbna are quoted by Abegg and (}oz, 1903; see also KoUiausch, 1904- 05;
BOttger, 1903, 1906.)
4*. X4'. ao*. 2S*. 42*. loo'.
Gms. AgCl per Liter 0.0014 0.0016 0.0020 0.0040 0.0218
More recent determinations are as follows:
f.
VYIDS. rVgV^l
per Liter.
Method.
Authority.
10
0.00089
Conductivity
(Kohlrausch, 1908.)
18
0.00150
Conductivity
(Melcher, 1910.)
21
0.00154
Colorimetric (See Note, p. 608)
(Whitby, 1910.)
25
0.00172
Analytical
(Glowczynski. 19x4.)
SO
0.00523
Conductivity
(Melcher, 19x0.)
100
0.02107
(<
(Melcher, 19x0.)
100
0.0217
Colorimetric
(Whitby, X9XO.)
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 dbh. 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
electroljrticaUy, dissolved in HN0| and titrated with o.ox n NH4SCN.
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, X908.)
8ILVEB CHLORIDE
606
Solubility op Silver Chloeide in Aqueous Ammonia Solutions at 25^
(Whitney and Mdcher, 1903.)
(Straub, zgiz.)
Gm. Mols.
Gm. Atoms
(kn. Mols.
Gm. Atoms
NH« (total)
A?
NHa (total) per
xooo Cms. Ii|0.
1000 Gms. H|0.
Solid Phase.
per Liter.
per Liter.
0.0282
O.OOI4I
0.0428
0.025
AgO
0.0288
0.00149
1.688
0.1308
u
0.0590
0.00304
3.782
0.372
tt
O.I18
0.00621
3-945
0.378
u
0.253
0.0140
S-io
0.574
u
0.397
0.0227
5-33
0.609
u
0.428
0.0249
5 545
0.633
<(
0.818
0.0514
6.26
0.754
" +aAga.3NU.
0.863
0.0541
6.52
0.775
sAgCaNU.
0.896
0.0569
8.28
0.848
((
0.909
0.0584
11.78
0.980
tt
0.961
0.0616
12.68
1.030
u
1. 991
0.147
12.96
1.090
tt
2.042
O.I5I
14.47
1.039
tt
Additional data for the above system at 25** are given by Bodl^nder and Fittig
(1901-02). These authors also give results showing the effect of KCl and of
AgNOt on the solubility of AgCl in aqueous ammonia. Determinations at 15^
are given by Bodl&nder (1892),
Solubility of Silver Chloride in Aqueous Solutions of:
Ammonia at 0**.
Monomethyl Amine at 11.5®.
Gany
, X899.)
Qarry.)
Gms. per zoo
Gms. Solution.
Gms. per xoo Gms. Solution.
NHaGas.
AgCl.
NHiGas.
AgCl.
NHtCH,. Aga.
1.45
0.49
28.16
6.50
1.78 0.16
2.94
1.36
29.80
7.09
4.44 0.62
5.60
3.44
30.19
725
5-51 0.83
6.24
4
32.43
587
7.66 1.32
11.77
4.68
34.56
4.77
13.70 3.29
16.36
5. 18
37.48
3.90
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, z86o.)
Solvent.
Aq. Ammonia of 0.998 Sp. Gr.
" 0.96 Sp. Gr.
" 0.986 Sp. Gr.
(t
t*
Gms. AgCl per
t .
zoo Gms. S<4vent.
s%
12
0.233
10%
18
7.84
80
1.49
3%
25
1.40
15%
25
7.58
607 SILVER CHLORIDE
Solubility op Silver Chloride in Aqueous Solutions op Methyl
Amine and op Ethyl Amine at 25**.
• (Bodlfiader and Eberlein, 1903; Wuth, 1902; Euler, 1903.)
Results for Methyl Amine. Results for Ethyl Amine.
Mols. per Liter.
Mols. per
Liter.
Total Base.
1. 017
AgCl.
0.0387
■■ ■ ^
Free Base.
0.940 (B.&E.)
Total Base.
0.483
AgCl.
0.0314
Free Base.
0.420(3. &E.)
0.93
0.508
0.203
0.102
0.195
0.0335
0.0178
0.0068
0.0036
0.00048
(E.)
0.472 (B.&E.)
0.189
0.0050 "
. . . (W.)
0.200
O.IOO
0.094
0.050
0.103
O.OII5
0.0062
0.0048
0.0029
0.00824
0.177
0.088
. . . (E.)
0.044 (B.&E.)
. . . (W.)
0.074
0.00042
• • •
0.0551
0.000235
it
...
0.020
0.00030
• • •
0.0127
O.OOOII4
• • •
Solubility of Silver Chloride in Aqueous Solutions op Ammonium
Chloride.
(Schierholz, 1890; see also Vogel, 1874; Hahn, 1877.)
Solubility at 15®. Solubility at Different Temperatures.
Gms. per 100 Gms. Solution.
t* *
NH4CI. AgCl.
15 26.31 0.276
40 " 0,329
60 " 0.421
80 " 0.592
90 " O.711
100 " 0.856
no " 1.053
Sp. Gr. of 26.31% NH4CI solution
at 15° =1.08.
One liter aq. sol. containing 0.00053 S^« NH4CI dissolves 0.001604 S™* AgCl
at25^
One liter aq. sol. containing 0.00530 gm. NH4CI dissolves 0.002379 gm. AgCl
at 25®. (Glowczynski, 19 14.)
Solubility op Silver Chloride in Aqueous Solutions op Ammonium
Chloride at 25®. (Forbes. X9ix.)
Gms. Equiv. per Liter. Gms. Equiv. per Liter. Gms. Equiv. per Liter.
Gms. per xoo Gms. Solution.
NH«a.
AgCl.
10
0.0050
14.29
0.0143
17.70
0.0354
19.23
0.0577
• 21.91
O.IIO
25.31
28.45
Sat. at ord. temp.
0.228
0.340(24.5)
9.157
NH4C1.
Ag. '
■NH4CI.
Ag.
NH4CI.
Ag.
0.513
0.000042
2.566
0.001425
4-777
0.0135
0.926
O.OOOII3
2.918
0.002160
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 AgNOt
to the chloride solution and observing the point of initial opalescence
Solubility op Silver Chloride in Aqueous Solutions op Aluminium
AND Ammonium Salts. (Vaknta; see also Cohn, 1895.)
Aq. Salt Solution.
Aluminium Thiocyanate
Ammonium Carbonate
" Thiocyanate
Thiosulfate
f.
Gms. AgCljper 100 Gms. Solvent
of Concentration:
1—
I : 100.
5 : 100.
xo : 100.
25
• • •
* ■ •
2.02
25
• • •
• • •
0.05
20
• • •
0.08
O.S4
20
0-57
1.32
392
Calc. by Cohn*
0.64
307
5-86
* See Note, p. 603.
8ILVEB CHLORIDE
608
SoLUBiLmr OF Silver CHLORroE in Aqueous Solutions op Barium
Chloride and of Calcium Chloride.
(Forbes, 19x1.)
Cms. Equhr. per Liter.
Cms. Equiv. per liter.
Aq. Sdution of: t*. BaCli
Ag.
Aq. Solutkm of: t*. CaCls
Ag.
Barium Chloride
u
tt
25
25
25
25
a " 2
1.248 0.000186 Caldum Chloride 25 3.264 0.001463
1. 610 0.000339 " 25 3.737 0.002182
2.676 0.001274 " 25 4.033 0.002802
3.260 0.002366 " 25 4-538 0.00417s
CaCl,
Calcium Chloride 25 1.748 0.000289
25 2.201 0.000501
25 2.741 0.000900
tt
tt
tt
tt
It
tt
25 5.005 0.005823
I 3.512 0.000964
25 3.320 0.001514
35 3.221 0.001806
Solubility of Silver Chloride in Aqueous Solutions of Hydro-.
chloric Acid at 25®.
(Forbes, 19x1.)
Gms. Equiv. per Liter.
llCl! ' Ag! '
0.649 0.000032
1.300 0.000126
I. 911 0.000266
Gms. EqiiJY' per Liter.
HCl. ' Ag! '
2.149 0.000374
2.975 0.000814
3.576 0.001358
Gms. Equiv. per Liter.
^lici! ^ Ag! '
4.182 0.002147
4. 735 0.003168
5.508 0.005126
The determinations of Forbes were made by gradually adding 0.25 n and o.oin
AgNOi to the chloride solution and observing the point of initial opalescence.
Oneliterof i per cent aq. HCl dissolve 0.0002gm.AgClat2I^ (Whitby, 'xo.)
" " 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. HCl 4- Aq.
I vol. Cone. HCl 4- 1 vol. HiO
Sat. HCl Sp. Gr. 1.165
tt
ti
Gm.1. AgCl
per Liter.
Solvent.
5
100 vol. sat. HCl + 10 vol. HiO
oLHiO 1.6
+ 20
2.98
+ 30 "
(at b. pt.) 5 . 60
+ 50 "
Gms. AgCl
per Liter.
0.56
0.18
0.09
003s
Solubility of Silver Chloride in Aqueous Solutions of Mercuric
Nitrate at 25®.
(Morse, 1902.)
Mols.
HgN0^(HNOt)
per Liter.
O.OIOO
Mols. AgCl
per Liter.
Gms. AgQ
per Liter.
Mols.
HgN0>(HN0,)
per Liter.
0.050
O.IOO
I
Mols. AgCl
per Liter.
Gna. Ag(3
per liter.
0.00914
0.01395
0.04810
1. 310
6.896
.0.00432 0.620
0.0125 0.00499 0.715
0.025 0.00690 0.990
^ Since HNOi 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 HNOt. Both crystallized and amorphous
silver chloride gave identical results.
6o9 SILVER CHLORIDE
Solubility op Silver Chloride in Aqueous Salt Solutions.
(Vogel; Hahn; Valenta )
CoDc. of Salt. t **.
Salt Solution.
Barium Chloride
Barium Chloride
Barium Sulphocyanide
Calcium Sulphocyanide
Calcium Chloride
Calciiun Chloride
Copper Chloride
Ferrous Chloride
Ferric Chloride
Manganese Chloride
Magnesiiun Chloride
Magnesium Chloride
Magnesium Chloride
Strontium Chloride
Zinc Chloride
Potassiiun Chloride
Potassium Chloride
Cms. AgQ per
xoo Cms. Solutioii.
27.32%
saturated
10 :ioo
10 : 100
41.26%
saturated
a
It
it
tt
50 :ioo
36.35%
saturated
((
24 -95%
5:100
5:100
Potassium Cyanide
Potassium Cyanide
Potassium Sulphocyanide 10:100
Sodium Chloride satxu-ated
Sodium Chloride 25 . 95%
245
ord. temp.
25
25
245
ord. temp.
245
((
tt
ti
25
245
ord. temp.
it
245
ord. temp.
19.6
as
25
25
ord. temp.
I0-6
O.OS7
0014
0.20
015
0571
0.093
0.053
0-169
0.006
0.013
0.50
0531
O.171
0.088
0.0134
O047S
0.0776
2-75
524
O.II
0.095
0.105
(H.)
(Vg.)
(VL)
(VI.)
(H.)
(Vg.)
(H.)
(H.)
(H.)
(H.)
(VI.)
(H.)
(Vg.)
(Vg.)
(H.)
(Vg.)
(H.)
(VI.)
(Cohn*)
(VI.)
(Vg.)
(H.)
See Note, p. 603.
Solubility of Silver Cm^ORioE in Aqueous Solutions of Nitric
Aero AT 25*.
(Glowczynski, 19x4.)
Mols. per Liter. Cms. per Liter.
HN0|.
0.0005
O.OOI
O.OI
0.30
i.5o(?)
AgCl.
1.15.10"*
1.19.10"*
I . 24 . 10"*
1.57.10-^
I. 71. 10"*
HNOk.
0.0315
0.063
0.630
18.9
94.5
AgCl.
0.001647
0.001705
0.00176
0.00225
0.00245
Solubility of Silver Cm^oiuDE in Aqueous Solutions of Potassium
Cm^oRTOE AT 25®.
(Forbes, 19x1.)
Cms. Equiy . per Liter. Cms. Equiv. per Liter.
Kci. "~Ai! ' ^KcT ""aJ; '
X.lll 0.00014X 2.850 0.001845
1.425 0.000235 3 081 0.002435
1. 713 0.000391 3.424 0.003602
2.022 0.000616 3.843 0.005725
2.396 0.001050 3.325 0.001734 (at x")
2.628 0.001390 2.955 0.002786(8*35")
(Glowo^nski, X9X4.)
Mols. per Liter.
KCI. ' AgCl.
3.i6.io~* 1. 28.10"*
6.32.10"* 1.52. 10"*
2.0.10 "^ 2.13.10"*
4.0.10 ~* 2.24.10"*
Cms, per Liter.
^KCT AgCl.
0.00236 0.001836
0.00471 0.002178
0.0149X 0.003052
0.02984 0.003209
The determinations of Glowcr^ki were made by the method described in
Note, on p. 605. The determinations of Forbes were made by gradually adding
0.25 n and 0.01 n AgNOt to the chloride solution and observmg the point of
mitial opalescence.
One liter 4 n aq. KCI dissolves 0.00637 gm. mol. = 0.915 gm. AgCI at 25®.
(Hellwig. 1900)
8ILVEB CHLORIDE
6io
Solubility of Silver Chloride in Aqueous Solutions op
Potassium Chloride at 15°.
(Scbierholz — Siuber. K. Akad. Wiss. (Viemia) zoi, ab. 8, '90.)
Grams
xoo Grams
tttion.
Grams
iZi
xoo Grams
£5!
10. 0
14.29
16.66
20.00
ution.
Aga.
0.000
0.004
0.008
0.020
KCl. A«a.
22.47 0.045
24.0 0.072
25.0 0.084
Sp. Gr. of 25% KCl soL,- 1179
Mixtures op Silver Chloride and Silver Hydroxide in Equi-
librium WITH Aq. Potassium Hydroxide Solutions at 25^.
(Noyes and Kohr — J. Am. Ch. Soc. 24. X144. 'oa.)
Normality Millimols per liter. Grama lyr Liter.
<rf J^OH. go! koh. kcT koh! Xga.
0-333 3414 347-S 0255 10.05 0.4896
0.065 0.598 65.0 0.0446 2.00 0.0828
Solubility of Silver Chloride in Aq. Sodium Chloride Solutions.
(Schierfaolz; Vogcl; Hahn.)
SolubUity at I5^
Gms. per 100 Gms.
Solution.
KaCl.
10 0
AgCl.
00025
14.29
18.18
0.0071
0.0182
21.98
23 -53
25.64
26.31
00439
0.0706
0.103
0.127
Solubility at Different Temperatures
A o Gms. AgCl per 100 Gm&
* SdutioQ in:
14% NaCl
36.3% NaCl.
IS
0.007
0.128
30
OOII
0.132
40
0.014
0.158
50
0023
0.184
70
0.042
0263
80
0.054
O.3IS
90
0.069
0.368
100
0.090
0.460
Sp.Gr. of 26.31% NaCl sol. « 1.207. 109 0107 (104°) 0.571
Solubility at 20**, 50°, and 90° (Calc. prom Original).
(Barlow — J. Am. Chem. Soc 28> 1446, '06.)
Gms. NaQ
per 100 cc.
Gms. AgCl dissolved per xoo cc.
Solution at:
Gms. NaQ
per 100 cc.
Solution.
"■5
Gms. AgO dissdvcd per xoo cc
Solution at:
Solution.
3-43
ao®. 50". 90";
0.00018 0.0016 0.0067
'ao«. 50°.
0.0031 00124
0.0436
4.60
0.00025 0.0025 O.OIOO
153
0.0090 O.OI9I
0.0732
S-7S
7.67
0.00047 0.0034 0.0135
0.00125 00058 0.0236
23.0
00313 0.0889
0.1706
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, 191 1.)
Gms. Equiv. per Liter.
Gms. Equiv. per Liter.
Gms. Equiv. per Liter.
' [NaCll.
[AgjXiO*'.
' [NaCU.
[Agjxio*;
(NaQl.
[AglXxo»;
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
0.24s
3.270
1.583
4-S3S
4.298
1. 871
0.348
3 471
1.897
5-039
6.039
6ii 8ILVEB CHLORIDK
Solubility of Silver Chloridb in Aq. Sodium Nitrate Solutions.
^^ Cms. per loo Cms. HjO. ^. Gms. per lop Gms. H|0.
I^aNOi. ^ AgCl. '
0.393 0.00096
0.787 0.00133
2.787 0.00253
(Mulder.)
One liter aq. 3 » AgNOs dissolves 0.0056 gm. mols. » 0.8 gm. AgCl at 25^.
(HeUwig, 1900.)
Solubility of Silver Chloride in Aqueous Sodium Sulfite Solutions
AT 25*.
(Luther and Leubner, 19x2.)
Gms. Formula Weight per Liter. Gms. Formula Wdght per Liter.
» .
KaNO).
AgQ. '
» .
5
0.787
0.00086
15-20
18
0.787
0.00146
a
30
0.787
0.00233
u
45-55
0.787
0.00399
SO,".
Ag'. '
SO,".
Ag'.
0.080
O.OII
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
0.140
0.478
0.057
0.937
0.142
The AgCl was prepared by precipitating dilute AgNOt with alkali chloride at
the b. pt. The resulting solid correspond^ 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.
(Vaknta; Cohn; Richards and Faber, 1899.)
Gms. AgCl per zoo Gms. Aq. Solutions of Concentration:
Salt Solution. V.
Sodium Sulfite 25
Sodium Thiosulfate 20
" " Calc by Cohn.'
Sodium Thiosulfate 35
Thiocarbamide 25
Thiocyanimine 25
* See Note, p. 603. f Gms. per zoo cc. solution (R. and F.).
Solubility of Silver Chloride in Aqueous Strontium Chloride at 25*.
(Forbes, zgzz.)
Gms. Equlv. per Liter. Gms. Equiv. per Liter. Gms. Equiv. per Liter.
z : zoo.
S:zoo.
zo : zoo.
Z5 : zoo.
90 : zoo.
• • •
• • •
0.44
• • •
0.95
0.40
0.38
2
1.83
4.10
5.50
5.02
6.10
6.41
m • •
• • ■
• « •
• • •
• • •
0.83
• • •
• » •
9.o8t
• ■ *
0.40
1.90
390
• • •
• • •
SrCI,.
2
AgXzo».
SrCl,
2
AgXzo«.
SrCl,.
2
AgXzo«.
0.550
0.033
1. 818
0.348
3-494
2.018
0.989
0.092
2.140
0.510
4.152
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 AgNOj to
the chloride solution and observing the point of initial opalescence.
One liter of 4.777 n ZnCU solution dissolves 0.000364 mol. AgCl at 25®.
(Forbes, zgzz.)
Fusion-point data are given for the following mixtures.
AgCl + Agl. (Monkemeyer, Z906.)
AgCl 4- AgiS. (Truthe, Z9Z2; Sandonnini, X9Z2.)
AgCl + NaCl. (Sackur, Z9Z3; Botta, zQzx; Sandonnini, xgiz, 1914.)
AgCl + TlCl. (Sandonnini, 191 x, 19x4.)
8ILVEB CHLORIDE
612
SOLUBILir
i OF Silver Chloridb
IN
Ptkidinb.
(KAhtenbcrg and Wittich, 1909.)
Gms. AgCI
t*. per xoo Gnu.
Psrridine.
Solid Phase.
f.
Gms. AffQ
per zoo Gms.
Pyridine.
Solid
Phase.
— 57 Eutec.
Aga.aQH.N+CAN
0
5-35
AgO
-49 0-77
AgaaCAN
10
317
M
-35 0-99
u
20
1. 91
M
—30 1.36
u
30
1.20
U
— 25 1.80
it
40
0.80
«
— 22 2.20
u
50
0.53
U
— tr. pt. 2 . 75
" +AgaCiH4N
60
0.403
«
-20 3.75
AgO-CAN
70
0.32
H
-18 3-85
tt
80
0.25
««
-10 435
n
90
0.22
U
- S S-OS
((
ICX)
0.18
M
- I 5.60
M
no
0.12
U
8ILVEB CHROHATE AgiCrO^.
One liter of water dissolves 0.026 gm. AgjCrO* at 18®, and 0.020 gm. at 25*.
(Abegg and Cox, 1903; Kohlrausch. 1904-05.)
One liter HtO dissolves 0.029 gm. Ag^CrO* at 25*^. (Schifer, 1905.)
One liter of H2O dissolves 0.0142 gm. AgiCrO* at 0.26®; 0.0225 gm. at 14.8®,
0.036 gm. at 30.7** and 0.084 S^^- ^^ 75**' (Kohliausch, X908.)
One liter HjO dissolves 0.0256 gm. at 18®, 0.0341 gm. at 27** and 0.0534 gm. at
50®, determined by a color imetric method (see Note, p. 608). (Whitby, 1910.)
Solubility of Silver Chromate in Aqueous Ammonia at 25*.
(Sherrill and Eaton, 1907.)
Mols. NH4OH per Liter o . oi o . 02 o . 04 o . 08
Mols. X 10' Ag2Cr04 per Liter 2 .004 4 . 169 8 . 595 17 . 58
Solubility of Silver Chromate in Aqueous Nitric Acid at 25®.
(Sherrill and Ruas, 1907.)
Mols. HNOi Milliatoms per Liter.
per Liter.
O.OI
0.015
0.02
0.025
0.03
0.04
0.05
3
3
4
4
5
5
6
Cr.
.157
•730
.177
.567
.200
.803
.380
Ag.
6.3IS
8.356
11.62
SoUd
Phase.
AgtCi04
per Liter.
0.06
0.07
0.075
0.08
0.10
0.13
0.14
One liter 65% aqueous alcohol dissolves 0.78 X lO"^ gms. equivalents =« 0.0129
gm. Ag2Cr04 at room temp. (?). (Guerini, 1912.)
«i
«
(I
«
tt
MUliatom!
» per Liter. Solid
Cr.
Ag. ' Phase.
6.833
. . . A&00«
7.333
...
7-477
14.85 « +Aa
7.260
15.45 "
S.647
19.01 "
4.293
23.89 «
3.948
25.63 "
Solubility of Silver Chromate in Aqueous Solutions of Nitrates at ioo*.
. (Carpenter, 1886.)
Solvent.
Water
Sodium Nitrate
Potassium Nitrate
Ammonium Nitrate
Magnesium Nitrate
Gms. Salt
Gms. Ag|CiO«
per 100 cc.
per xoo cc.
HaO.
Soltttbn.
0
0.064
SO
0.064
SO
0.192
SO
0.320
SO
0.256
Milluttonu per
Liter.
Cr.
Ag.
32.20
S-390
25.06 .
6. 131
20.21
7.148
13 -59
9 529
II. 10
II. I
•
II. I
II. I
U M
II II
II
II
613 SILVER CHROBIATB
SILVER (Di) CHROBCATE AgtCnOr.
One liter of aqueous solution contains 0.00019 gm. mol. or 0.083 gm. AgtCriO?
at 15*^. (Mayer, 19030
Solubility of Silver Dichromatb in Aqueous Nitric Acid at 25^
(Sherrill and Russ, 1907.)
O 32.20 S-390 A«Ci04+Ag,CrA
O.OI
0.02
0.04
0.06 II. 10 II. I AftCrA
0.08
0.08+0.1 AgNOs 6.625
At the lower concentrations some of the dichromate is converted into solid
chromate.
SILVER CITRATE CeHtOrAg,.
100 gms. HaO dissolve 0.0277 gm. CeHsOrAgt at i8^ and 0.0284 fi^- ^t 25°.
(Partheil and Httbner, 1903.)
SILVER CYANIDE AgCN.
One liter of aqueous solution contains 0.000043 S™* AgCN at 17.5^ and 0.00022
gm. at 20** (by Conductivity Method). (Abegg and Cox; Btfttger, 1903.)
Solubility of Silver Cyanide in Aqueous Ammonia Solutions.
(Longi, Z883.)
100 gms. aq. ammonia of 0.998 Sp. Gr. = 5%, dissolve 0.232 gm. AgCN at 12®.
100 gms. aq. ammoitia of 0.96 Sp. Gr. = 10%^ dissolve 0.542 gm. AgCN at 18*.
One' liter aq. 3 n AgNOt dissolves 0.0091 gm. mol. = 1.2 16 gm. AgCN at 25®.
(Hellwig. 1900.)
Fusion-point data for mixtures of AgCN + NaCN are given by Truthe (1912).
SILVER FERRICYANIDE AgsFeCN..
One liter HiO dissolves 0.00066 gm. AgtFeCN« at 20®. See Note, p. 608.
(Whitby, X9ZO.)
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. HiO dissolve 4.7 gms. at o®, and 7.4 gms. at 16". (Fronmoller, 1878.)
SILVER rLUORIDE AgF.2HsO.
Solubility in Water.
(Guntz and Gtintz. Jr., 1914.)
r.
Gms. AgFper
100 Gms. HfO.
Solid Phase.
f.
Gms. AgF per
xoo Gms. afi.
Solid PhtM
— 14.2 Eutec.
60
Ice+AgF.4HiO
25
179 s
AgF.3H,0
+ 18. s
I6S
AgF-*H,0
28. s
2IS
M
18.6s
169.5
" +AgF.2H/)
32
193
<(
20
172
AgF.sH^
39. S
222
" +AgF
24
178
u
108
20s
AgF
Two unstable hydrates, AgF.HjO and 3AgF.5HjO were also obtained.
100 gms. HsO dissolve 181 .8 gms. AgF at 15.8^, du.% of Sat. Sol. «■ 2.61 . (Goce, 1870.)
SILVER nUOBIDK
614
Solubility of Silver Fluoridb in Aqueous Solutions of Hydro-
fluoric Acid at &* and at 24^.
(Guntz and Guntz, Jr., 19x4.)
Results ,. Results at 24^
Cms. per 100
Gms. HiO.'
Solid PhtM.
Gnu. per IOC
t Cms. Bfi.
SnlMPhHe.
A«F.
HF.
AgF.
HF.
87 -5
0.40
AgF.4H|0
178
0
AsF.9HiO
89.4
2.60
««
178.5
1-73
«(
93-8
3-97
If
177-65
5-42
II
118. s
9.60
u
179-5
10
M
156
14
" +A«F.aIV)
189. s
13-4
M
1 59
17.2
AgF.3H|0
191 -5
14.3
" +A«F(?)
i8s
24
«<
207
0 15
3 AgF.sHdO
189
25-7
A«F
206.2
I. 25
M
188
29s
M
202.5
7-9
II
196
39-8
l<
198.6
12.65
M
142. 1
52
AcF.2H^
195-5
II. 7
AgF.H^
121.7s
57-2
u
194-5
13
<i
94-93
66.57
I*
189.5
18.8
3AgF.5Hrf)+AgFC?)
173-75
0.4
sAgF.sEfi
193
36.6
A«F
174
3.6
«<
193 -5
16
Additional determinations at other temperatures are given.
SILVER rULBONATE CAgs(NOi)CN.
One liter of aqueous solution contains 0.075 S™< CtAgtNtOs at 13°, and 0.180
gm. at 30"* (Holknum. 1896.)
SILVER HEPTOATE (Onanthylate) AgCrHnOs.
Solubility in Water.
(Landau. 1893; Altachul, 1896.)
r.
o
10
20
30
40
Gms. AgCiHi/)^ per xoo Gms. H^.
/ *
0 . 063 5 (Landau) 0 . 0436 (Altachul)
0.0817 0.0494
0.1007 0.0555
0.1206 0.0617
0.1420 0.0714
f.
50
60
70
80
Gms. AgC-iHtfif per xoo Gms. HjO.
, * ,
0.1652 (Landau) 0 . 08 58 (Altachul)
0.1906 0.1036
0.2185 o.issi
0.2495 0.1688
SILVER lODATE AglO,.
One liter of aqueous solution contains 0.04 gm. or 0.00014 S™- n^ol. at 18*^-20^,
and 0.05334 K^' or 0.000189 gm. mol. at 25 .
(Longi; BOttger; Kohlrauach; Noycs and Kohr, i903.)
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. AsIOi per
liter at 20^. Determinations reported by Sammet (1905) made by a chain cell
method, gave 0.0611 gm. AglOi per liter at 25** and 0.1849 gm. at 6o^
One liter of HiO dissolves 0.0275 gm. AglOi at 9.43®, 0.039 gm. at 18.4® and
0.0539 gm. at 26.6^. (Kohlrauach, 1908.)
Solubility of Silver Iodate in Aqueous Solutions of Ammonia and
OF Nitric Acid at 25®.
(Longi. 1883.)
100 gms. aq. ammonia of 0.998 Sp. Gr.
100 gms. aq. ammonia of 0.96 Sp. Gr. -
100 gms. aq. nitric acid of 1.21 Sp. Gr.
= 5% dissolve 2.36 gms. AglOi.
> 10% dissolve 45.41 gms. AglOs.
"" 35% dissolve 0.096 gm. i^IOt.
6i5 8ILVEB lODATE
Solubility of Silver Iodatb in Aqueous Solutions of Nitric Acid at 25®.
(Hill and Simmons, 1909.)
Normality of Gms. AglO^ Normali^ of Gms. AglO^
Aq. HNOs. per Liter. Aq. HNO^. per Liter.
o 0.0503 I 0.2067
0.125 0.0864 2 0.3319
0.250 0.1075 4 0.6985
0.500 0.1414 8 1-587
The solubility of the amorphous modification of AglOi 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 20^-25^
(Average of several determinations by Kohlrausch, Ab^^ and Cox, etc., Holleman gives mgher figures.)
One liter of water dissolves 0.0000253 gm. Agl at 60**, determined by a chain
cell method (Sammet, 1905). This author also gives data for the solubility of
Agl in I » and o.i n KI solutions at 60**.
Solubility of Silver Iodide in Aqueous Ammonia.
«^'SL2Aq. Xl^lk. t-. Gms^^l ^^^^
7 0.971 16 0.045 (Ladenburg, 1902.)
10 0.960 12 0.035 (Longi, 1883.)
20 0.926 16 0.166 (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. H^0i)t Mols. Agl
per Liter. per Liter.
o.oio 0.00340
0.0125 0.00358
0.025 0.00476
Since HNOi was present in all cases its influence on tlie solubility was examined.
It was found that no appreciable differences were obtained with concentrations
varying between o.i and 2 n HNOs. Both crystallized and amorphous silver
iodide gave identical results.
Solubility op Silver Iodide in Aqueous Solutions of Potassium
Iodide and of Silver Nitrate at 25®.
(Hellwig, 1900.)
In Aq. KI Solutions. In Aq. AgNOs Solutions.
Gms. Agl
Mols. H9(N0i),
Mols. Agl per
Gms. Agl
per liter.
per Liter.
Liter, j
per Liter.
0.800
0.050
0.00740
1.737
0.841
O.IOO
O.OI161
2.730
1. 118
I
p. 10700
25.160
Mob. KT
Mols. Agl
Gms. Agl
Mols. AgNOi
Mols. Agl
Gms. Agl
Solid "
per Liter.
per Liter.
per Liter.
per Liter.
per Liter.
per Liter.
Phase.
0.33s
0.000363
0.0853
0.20
0.000289
0.068
Agl
0.586
0.00218
0.512
0.3s
0.000532
O.I2I
«<
0.734
0.0044
1.032
0.50
0.00127
0.299
«
1.008
O.OI41
3.32
0.70
0.00362
0.850
M
1. 018
0.0148
3.47
I. 215
O.OI31
3.08
Ag.INQ,
1.406
0.0535
"•55
1.63
0.0267
6.26
u
1.486
0.0658
15.46
2.04
0.0458
10.9
M
1.6304
0.102
24.01
2-54
0.0678
16. 1
Ag,I(NO,),
1.937
0.198
46.42
3. 75
O.141
33.2
u
4.69
0.227
53.2
«
5.90
0.362
85
M
8ILVEB lODmS
6i6
Solubility of Silver Iodide in Aqueous Salt Solutions.
(Valenta, 2894; Cohn, 1895.)
Aq. Sdt. SoltttioiL t*.
Sodium Thiosulfate 20
" " CalclvCohn*
Potassium Cyanide 25
" " Calc.lv Cohn*
Sodium Sulfite 25
Ammonium Thioc^anate 20
Calcium
Barium "
Aluminium "
Thiocarbamide •
Thiocyanime
25
25
25
25
25
Gms. Agl per xoo Cms. Aq. Sol. of Conoentxaticm:
O
O
xoo.
03
623
5 : 100.
0.15
2.996
8.28
8.568
• • •
0.02
0.008 0.05
See Note, p. 603.
10 : 100.
0.30
5-726
O.OI
0.08
0.03
0.02
0.02
0.79
0.09
15 : 100.
0.40
8.218
013
ao
O
ID
xoo.
60
493
02
Solubility of Silver lonros in Aqueous Solutions of Sodium Cmx>RiDB,
Potassium Bromide and of Potassium Iodide at 15**.
(Schierholz, X890.)
In Sodium Chloride.
Cms. per 100 Gms. Solutioo.
NaQ.
26.31
25.00
Agl.
0.0244
0.00072
In Potassium Bromide.
Gms. per xoo Gms. Solution.
KBr
30.77
Agl
o . 132
In Potassium Iodide.
Gms. per 100
Gms
. Soludoa.
Kl.
Agl.
59.16
53-13
57 15
40.0
50.0
25.0
40.0
13.0
33-3
7-33
25.0
2-75
21.74
I 576
20.0
0.80
100 gms. sat. silver nitrate solution dissolve 2.3 gms. Agl at il^ and 12.3 gms.
at b. pt.
100 gms. pyridine dissolve 0.10 gm. Agl at lo^ and 8.60 gms. at 121^
(von Lasacynski, 1894.)
Solubility of Silver loDms in Aqueous Sodium Iodide at 25^
(Krym, 1909.)
Nal.
-^ST-
Solid Phaae.
Nal. Agl.
Solid Phaae.
59 29
21.21
Agl
226 120.9
AgI2faI.3iH^+NaI
67.47
28.52
II
222.7 112. I
Nal
134. 1
99-54
II
214.7 90.84
II
156.9
124.6
fi
203.9 59.48
M
179.8
150
" +AgI.NaI.3|H/)
194.5 . 31.10
(4
196.3
134.8
AgI.NaI.3iH,0
185.52 0
M
223.7
122
II
The above table was calculated from the original results which are expressed in
mols. per 1000 mols. HsO.
Fusion-point data for mixtures of Agl + Hglj are given by Steger (1903).
Results for Agl + Nal are given by Sandonnini and Scarpa (I9I3)-
6i7 SILVEB LAT7RATE
SILVER LATTRATE, BCTBI8TATE, PALMITATE and STEARATE
Solubility of bach, Determined Separately, in Water and Other
Solvents at Several Temperatures.
(Jacobson and Holmes, 19x6.)
Gms. eadb Salt per 100 Gms. Solvent.
Solvent. t*. / ^
Laurate. Myristate. Palmitate. Stearate.
Water 35 ... 0.007 0.004 0.004
n
50 ... 0.007 0.006 0.004
Abs. Ethyl Alcohol 25 0.009 0.008 0.007 0.007
" " 50 0.009 0.008 0.007 0.007
Methyl Alcohol 15 0.074 0.063 0.060 0.051
25 0.072 0.067 O.OS9 0.052
35 0.078 0.071 0.062 0.055
50 0.083 0.073 0.066 0.060
Ether 15 o.oio 0.009 0.009 0.007
tt u
SILVEB LEVULINATE (Acetyl propionate) CHi.COCHsCHiCOOAg.
Solubility in Water.
(Fuicht and Lieben, 1909.)
Ao Gms. per xoo 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
SILVEB MALATE C4H40»Agi.
100 gms. HsO dissolve 0.0119 gms. at i8^ and 0.1216 gm. at 25^
(Partheil and Habner» 1903.)
SILVEB NITBATE AgNO,.
Solubility in Water.
(Etard, 1894; Kremers, 1854; Tilden and Shenstone, 1884.)
^ Gms. AgNOi per loo Gms. Gms. AgNOi per 100 Gms.
Solution. Water. * Solution. Water.
— 5 48 (Etard) 50 79 (Etard) 82 455
o 53 55 122 60 81.5 84 525
10 62 63 170 80 85.5 87 669
20 68 69 222 100 88.5 9oi 952
25 70.5 72 257 120 91 95 1900
30 72.5 75 300 140 935
40 7^5 79 376 160 95
100 gms. sat. aq. solution contain 47.1 gms. AgNOt at —7.3® (— Eutectic).
(Middlebers, 1903.)
100 gms. sat. aq. sol. contain 65.5 gms. AgNOs at 15.5^ (Greenish and Smith, 1903.)
100 gms. sat. aq. sol. contain 73 gms. AgNOt at 30^. (Schreinemakers and de Baat, x9zoa.)
Solubility of Silver Nitrate in Aqueous Nitric Acid at 25®.
(Masson, 29x1.)
Gm. Mols.^ per Liter. Gms. AgNO,
<^ of Sat.
Gm. Mob
I. per Liter.
Sol.
HN0».
AgNOi.
2.3921
0
10.31
2.2754
0.4042
9.36
2.1243
0.962
8.08
X.9402
1.698
6.54
T . 7052
2.834
4- 526
per Liter.
Sol.
HNO,.
AgNO,.
per Liter.
1752
1.4980
4.497
2.590
440.1
1 591
1.419s
S.992
1.698
288.6
1373
I. 3818
8.84
0.843
143.2
nil
1.3976
12.53
0.347
58.96
769.1
100 gms. 2HNOj.3H«0 dissolve 3.33 gms. AgNOi at 20®, and 16.6 gms. at 100®.
100 gms. cone. HNOi dissolve 0.2 gm. AgNOs. (Schultz, x86o.)
SILVER NITRATE 6i8
Solubility of Mixed Crystals of Silver Nitrate and Sodium Nitrate
IN Aqueous Ethyl Alcohol.
(Hiflsink, 1900.)
Results at 25*^ in Results at 50^ in
Aq. CiHtOH of <^ = 0.945 (37 wt. %). Aq. CAOH of dv = 0.859 (75 wt. %).
Gms. per xoo
Wt. per cent in
Cms. per xoo
Wt. per cent in
Gms.
Sol.
Mix Crystals.
Gms.
Sol.
Mix Crystals.
' AcNOs.
NaNO»:
"AgNOt. NaNOs
AgNOi.
NaNdft.
AgNOft. NaNOft
47-32
00
100 0.0
29.78
0.0
100 0.0
44.01
8.78
99.1 0.9
27.9
2-5
99-5 05
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 57-1
24.56
24.82
27.6 72.4
18.3
71
31.0 69.0
8.02
26.41
9.9 90.1
9-5
8.3
17-5 82.5
0.0
26.77
CO 100. 0
0.0
8.54
CO lOO.O
Very extensive data for equilibrium in the system silver nitrate, succinic acid
nitrile and water are given by Middelbere (1903). This author first gives data
for the ternary systems and then results tor isotherms of the ternary system at
o®, 12**, 20**, 25® and 26.^®. A number of determinations for higher temperatures
are also given. The following compounds of succinic nitrile and silver nitrate
were identified: C,H4(CN)2.4AgNa. C2H4(CN),.2AgNO,, C,H4(CN),.AgN0,.
2C,H4(CN),.AgNO,.H,0, and 4l2C,H4(CN),.AgNO,]H,0. 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. AgNOt at 19^
100 gms. abs. ethyl alcohol dissolve 3.10 gms. AgNOs at 19^
Solubility of Silver Nitrate in Aqueous Ethyl Alcohol.
(Eder, 1878.)
Sp. Gr.of Aq.
Alcoholic
Mixture.
Volume
Gms. AgNOi
per xoo
Gms. A
q. Alcohol al
per cent
Alcohol.
' r^.
so*.
75".
0.815
95
3-8
7-3
18.3
0863
80
10.3
• • 1
42.0
0.889
70
22.1
• •
• • •
0.912
60
305
S8.
I
89.0
0-933
50
35-8
• •
« • •
0.951
40
56.4
98
3
160.0
0.964
30
73-7
m •
• • •
0-975
20
107.0
214
0
340 0
0.986
10
158.0
• • t
• • •
100 gms. of a mixture of i vol. (95%) alcohol + i vol. ether dissolve 1.6 gms.
AgNO, at I5^
100 gms. of a mixture of 2 vols. (95%) alcohol + i vol. ether dissolve 2.3 gms.
AgNO, at 15^
100 gms. H2O sat. with ether dissolve 88.4 gms. AgNOi at 15 . (Eder. 1878.)
100 gms. acetone dissolve 0.35 gm. AgNOi at 14®, and 0.44 gm. at 18**.
(von Lasczynski, 1894; Naumann, 1904^
6i9
SILVER NITRATE
Solubility of Silver Nitrate in Several Solvents.
Solvent.
f.
Gms. per xoo Gms.
Solvent.
Authority.
Acetonitrile (anhirdrous)
18
290
(Naumann and Schier, i9X4*)
It
ord. temp.
about 150
(SchoU and Steinkopf. 1906.)
Benzonitrile
18
about 105
(Naumann, 19x4.)
Benzene
35
0.022
(Linebaxger, 1895.)
«
40.5
0.044
Hydrazine (anhydrous)
ord. temp.
I (with decomp.) (Webh and Bioderaon, 19x5.)
Solubility of Silver Nitrate in
Pyridine.
GnM. AgNOk
Gms. AgNOk
f. pel
r 100 Cms.
CAN.
Solid Pfaaae.
r.
per xoo Gms.
r,H,N.
SoUd Phase.
—48.5 m. pt
, 0
C«N
45
62.26 A«NQ,.3Cya«N
-50.5
3
«
46
63.09
II
-53
6
tt
47
66.35
II
-59
9
It
48
70.85
II
—65 Eutec.
...
«+a«no,.6C»h,n 48 • 5 tr.
pt. . . .
"+A«NO,.aCI^N
-51.25
II. I
AgN0k.6C|HcN
45
69.85
AgN0|.2C|H»N
-44
II. 7
«
50
72.25
II
-40
12.2
u
60
78.60
II
-35
12.6
tt
70
89.10
II
-30
13.9
u
80
121. 21
M
-25
17.6
tt
87
215.02
II
— 24 tr. pt.
m • •
"+AgN0,.3C:,H,N 80
228.5
II
— 22
18.8
AgN0|.3C|H|N
\ 74
230.6
M
— 10
20.03
II
74
225.4
M
0
22.34
II
80
230- 4
II
+10
27.21
II
87
237 I
l(
20
33.64
II
90
241.9
il
30
40.86
II
100
253.8
li
40
53- 52
II
no
271.4
M
Fusion-point data for mixtures of AgNOi + TlNOj are given by van Eyk (1905).
SILVER NITRITE AgNOi.
Solubility in Water.
(Creighton
and Ward, X9X5.)
Gms. AgNOi
t*
Gms. AgNOi
*•
(}ms. AgNOb
per Liter.
per Liter.
V •
per Liter.
1.55
20
3.40
40
7.15
2.20
25
4.14
50
9.95
2.75
30
5
60
13.63
r.
o
10
15
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 Aqueous Solutions of Silver Nitrate at 18®.
(Naumann and Rucker, X905.)
Mob, per Liter.
AgNQi.
0.0000
AgNOj.
0.02067
0.00258 0.01975
0.00517 0.01900
0.01033 0.01689
Grams per Liter.
AgNOs. AgNOs.
0.000 3.184
0439 3 042
0.878 2.926
1.756 2.601
Mots, per liter
Ai(NOft. AgNOj."
0.02067 0.01435
0.04134 O.OI168
0.08268 0.00961
Grams per Liter.
AgNOs. AgNOs.
3.512 2.201
7.024 1.799
14.048 1.480
8ILVBB NlT&m 630
Solubility of Silver Nitrite in Aqueous Solutions of Silver Nitrate
AND OF Potassium Nitrite at 25®.
(CreightoD and Ward, 1915.)
In Aqueous AgNOi. In Aqueous KNCX.
Mob. AgSOi DiMolvcd AgNCH Pcr Liter. Moh. KNO^. Diawlved AgNO^ per Liter.
P« Liter. ' u^. ^^ Cms. ' per Liter. ' Mob. ' GmZ
o 0.0269 4- 13s o 0.0269 4.13s
0.00258 0.0260 3-991 0.00258 0.0259 3.974
0.00588 0.0244 3.73s 0.00588 0.0249 3.820
O.OII77 0.0224 3.432 O.OII77 0.0232 3.560
0.02355 0.0192 2.943 0.02355 0.0203 3. 119
0.04710 0.0164 2.498 0.04710 O.O181 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 NaNOt dissolves 3.185 gms. AgNOt at 25^.
" " " 0.2011 " " 3.016 "
" " " o.2onNaNOi " 4.956 "
(Ley aod Schacfer, 1906; see abo p. 66a)
100 gms. HsO sat. with both salts contain 10.9 gms. AgNOi + 78.3 gms.
Sr(NCV)t at 14®. (Oswald, xgia, 1914.)
100 gms. acetonitrile dissolve about 23 gms. AgNOt at ord. temp, and about
40 gms. at the boiling-point (81.6*^). (SchoU and Steinkopf, 1906.)
SILVER OXALATE Ag,C,0«.
One liter H|0 dissolves 0.0378 gm. AgtCtOi at 21°, see Note, p. 608.
(Whitby, 1910.)
One liter HtO dissolves 0.0416 gm. AgtCiOi at 25^ Conductivity method.
(Schifer, 1905.)
One liter H|0 dissolves 0.0265 gm. AgtCiOi at 9.72°, 0.034' gm. at 18.5** and
0.043 gm. at 26.9^. (Kohhausch. 1908.)
Solubility of Silver Oxalate in Aqueous Nitric Aao at 25^.
(Hill and Simmons, 1909.)
(jms. Normal- Per cent v_ .# Gms.
AK,Cp4. ityof Cone. s5'Sl A&C/)*
per Liter. Aq. HNO,. of HNO.. ^at- »«. perUtcr.
1.345 4.017 22.37 1.141S I7-"
2.189 5.564 29.84 I. 1996 29.96
3.720 5.83 31-085 I. 2162 33-88
7.170
SILVER OXIDE Ag,0.
One liter of HsO dissolves 0.021 gm. at 20°, and 0.025 Rni. at 25^
(Noyes and Ronr; Bdttger; Abegs and Cox.)
One liter HiO'dissolves 0.02 1 5 gm. AgiO at 20*^. (See Note, p. 608.) (Whitby, 19x0)
Solubility op Silver Oxide in Water.
(Rebiere, 19x5.)
- -_^. . * T» ^' « .. *. 1 (*"• MoU. AgiO per Liter. Gms. Ag|0 per Liter.
Method of Preparation of the Sample. < , , ^ , , > *^ . " , . »
At as*. At so*. At as". At so*.
By action of NaOH on AgNOj 2.16,. lo"^ 2.97.10"^ o . 050 o . oi59 1
By action of Ba(OH)i on AgNQi 2. 23. 10"* 3.09. 10"* 0.0519 0.0719
By action of KOH on AgCl 2.32. 10"* 3.55. 10"* 0.0538 0.0825
By action of KOH on AgtCOk 2 . 95 . 10"* 3 . 89 . 10"* o. 0680 o. 0904
Solubility op Silver Oxide in Aqueous Ammonia at 25°.
(Whitney and Melcher, 1903.)
Mob. NHa Gm. Atoms A« Mols. NIL Gm.' Atoms A« Mols. NIL Gm. Atoms Ac
CToUl) per Liter. per Liter. (ToUl) per Liter. per Liter. (Total) per Liter. per Liter.
0.220 0.0658 0.733 0.224 I. 147 0-343
0.469 0.134 0.876 0.257 1.498 0.454
•-.684 0.205 0.915 0.276 1.522 0.470
Normal-
Percent
Sat. SoL
ity of
Aq.HNQ|.
Cone,
of HNQi.
0.2517
I. 574
1.0080
0.5025
3117
I. 0186
0.9806
6.017
1.0339
1.040
11.476
1.0647
621
SILVER OXIDE
Solubility of Silver Oxidb in Aqueous Solutions of Ethyl Amine and
OF Methyl Amine at I8^
(Euler, 1903.)
In Aqueous Ethyl Amine. In Aqueous Methyl Amine.
Nonnality of Nonnality of Nonnality of ' NonnaK^ of
Aq. Amine. Dissolved Ag. Aq. Axnme. Dissolved Ag.
o.ioo 0.0322 o.ioo 0.0221
0.50 0.160 0.500 o. 118
I 0.314 I 0.228
SILVER PERMANQANATE AgMnO^.
100 gms, cold water dissolve 0.92 gm.: hot water dissolves more.
(Mitscherlicfa, 1831.)
SILVER PHOSPHATE Ag,PO«.
One liter of water dissolves 0.00644 gm. at 20^
SILVER PROPIONATE CiHtCOOAg.
Solubility in Water.
(RanpeiiBttaiidi, 1885; Arrbeniua, 1893; Goldschmidt, 1898.)
Gms. (VHiO^ *• Gms. (VHAAg
per Liter. * per Liter.
5.12 20 8.36(8.48) 50
6.78 25 9.06 70
8.36(A) 30 9.93(9.70) 80
(Bflttger, 1903.)
v:
O
10
18.2
f.
Giiis.CiHAAg
per Liter.
13.35
17.64
20.30
Solubility of Silver Propionate in Aqueous Solutions of:
(Axxfaenius.)
Silver Nitrate at I9.7".
Mols. per Liter. Gms. per Liter.
Sodium Propionate at 18.2^.
Mols. per Liter. Gms. per Liter.
AgNOa. C»EI»0|A«.
o 0.0471
0.0133 O.04IS
0.0267 0.0379
0.0533 0.0307
O.IOO 0.0222
AgNOt.
O
2.289
4.577
9 059
16.997
CmOiAg.
8.519
7.511
6.86
5.556
4.019
o
0.0167
0.0333
0.0667
o. 1333
0.2667
0.5000
CAQiAg.
0.0462
0.0393
0.0345
0.0258
0.0I9I
O.OI3I
O.OIOI
CAQiNa. CAO^Ag.
O
1.607
3.215
6.429
12.859
25.718
48.77
8.362
7. 114
6.244
4.670
3.456
2.371
1.828
SILVER SALICYLATE C«H4.0H.C00Ag 1,2.
One liter of aqueous solution contains 0.95 gm. at 23^
SILVER SUCCINATE C«H«04Agi.
100 gms. H|0 dissolve 0.0176 gm. at i8^ and 0.0199 S^* ^t 2g^
SILVER SX7LFATE Ag,SOi.
(HoUemaiiJtSga.)
and HUbner, 19013.)
Solubility
IN Water.
(Barre.
1911.)
f.
Gms. A«sSO«
zoo Gms. Sat.
^
f.
Gms. Ag|S04
zoo Gms. Sat.
per
SoL
f.
Gms. AASO4 per
zoo Gms. Sat. SoL
0
10
0.57
0.69
30
40
0.88
0.97
70
80
I. 21
1.28
20
25
0.79
0.834
50
60
1.05
1. 14
90
100
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 Iiarkins
(191 1 ). Earlier determinations, differing somewhat from the above, are given by
Euler (1904), Wright and Thompson (1884), Wentzel ( ) and Drucker (1901}.
8ILVXB SULFATE
622
Solubility of Silver Sulfate in Aqueous Solutions
Sulfate.
(Bane, zgii.)
Results at 33^ Results at 5I^ Results at 75^.
Gms. per zoo Cms. Gms. per zoo Gms. Gms. per zoo Gnu.
&Lt. Sol. Sat. Sol. Sat. Sol.
OF AlOf ONIUIC
Results at loo^
Gms. per zoo Gms.
Sat.SoL
(NH«),SO«. Ag^4.
8.85 I.IOI
15-90 I-33I
22.22 1.500
27-25 1-585
30.80 I. 619
35.88 1.627
39.46 1.600
43-22 1.557
(NH4),S04. A&SO4.
8.90 1.362
16.27 1.680
22.43 1-887
32.10 2.061
35-38 2.095
39.03 2.082
42.37 2.055
45.05 2.026
(NH4),S04. A«|S04.
8.80 1.758
15-23 2.155
22.30 2.490
28.25 2.734
32 2.823
35.82 2.889
41.16 2.929
46.46 2.902
(NH()tS04. Ag^SQi.
9.23 2.221
15 2.626
22.01 3.075
27 3325
34.90 3-663
38.70 3-772
44.15 3 854
47.63 3.867
A series of determinatioiis at 16.5*^ is also given.
Solubility of Silver Sulfate in Aqueous Nitric Acid at 25*
(Hill and Simmons, Z909.)
Normality
of Aq.
HNOa.
O
1.0046
2.0452
4.017
Percent
Cone, of Aq.
HNO,.
O
6.154
12.005
22.37
Sat. Sol.
1.0054
1. 061
I. 1069
I.1871
Gms. Af,S04
per Liter.
8.35
34.086
49.010
71.166
Normality
of Aq.
HNQi.
4.209
5 564
8.487
10.034
Percent
Cone, of Aq.
HNO^
23-33
29.84
42.37
48.77
Sat. SoL
I . 1956
I . 2456
1.3326
1.3676
Gms. A^aSO«
per Liter.
73.212
84.609
94.671
90.806
Solubility of Silver Sulfate in Aqueous Solutions of Acids and
Salts at 25®.
(Swan, z899.)
Acid or
Gm. Equiv.
Gms. Dissolved
Arid or
Gm. Equiv.
Gms. Dissolved
Salt.
per liter.
AgsS04 per Liter.
Salt.
per Liter.
AgsS0« per Liter.
HNO,
0
8.
41
HaSO/
0
8.41
((
0.01589
9-33
u
0.02902
8.55
((
0.03178
10.
18
u
0.05802
8.68
u
0.06357
II.
83
a
0.10526
8.86
KHS04
0.05264
8.
13
KtS04
0.02718
7-93
«
0.10526
8.
07
u
0.05434
7.68
Solubility of Silver Sulfate in Aqueous Solutions of
Salts at 25*.
(Harkins. zgiz.)
Salt.
Gm. Equiv.
per Liter.
Sat!V>l.
Gms.
Salt.
Gm. Equiv.
Salt
per Liter.
^'^^^P&S..
KNO*
0
• • »
8.344
AgNO,
0.09961
I. 0137 2.644
((
0.024914
1.0072
8.996
K,S04
0.025024
1.0064 7.899
((
0.049774
1.0092
9.531
((
0.050044
1.0079 7.694
n
0.09987
1.0034
10.435
u
O.IOO
1.0112 7.49
Mg(NO,),
0.024764
1.0073
9.267
u
0.20003
1. 0180 7.531
t<
0.049595
1.0094
10.029
MgSOi
0.020022
I. 0061 8.140
It
0.09946
I. 0133
"334
((
0.050069
1.0079 7.941
AgNQ,
0.024961
1.0065
6.095
((
0.10004
I. 0105 7.740
((
0. 04986
1.0084
4.487
u
0.20005
I. 0164 7.733
One liter of aqueous solution in contact with a mixture of silver sulfate and
silver acetate contains 3.95 gms. AgiSOi + 8.30 gms. CHiCOOAg at 17**. Sp. Gr.
of solution B 1.0094. (Eulcr, 1904.)
623
SILVER 8X7LFATE
SoLUBiUTT OP Silver Sulfate at 35^ in Aqueous Solutions of:
(Dnicker, 1901.)
Sulfuric Add.
Mok. per Liter. Gms. per Liter.
AaSOi. H1SO4:
8. II 0.98
8.23 1.96
8. 45 4.90
8.58 9.8Z
Potassium Sulfate.
Mob. per Liter. Gnu. per Liter.
AaS0«. h^soT.
0.0260 0.02
0.0264 0.04
0.0271 O.IO
0.0275 0.20
Ag9S04. K«S0«.
0.0246 0.02
0.0236 0.04
0.0231 O.IO
0.0232 0.20
AgaS0«. K«SO«.
7.67 1.74
736 3-49
7.20 8.72
7.24 17.44
Solubility of Silver Sulfate in Aqueous Potassium Sulfate Solutions.
(Barre, 1911.)
Results at 33^ Results at 51*
Gms. per xoo Gms.
. j)er
Sat.
Gms.
Sol.
KtSO«.
3.22
S.62
8.37
10.41
11.80
A«tS04.
0.863
0.940
1. 046
1. 117
1. 177
K«S04.
3.20
5.61
8.40
10.55
13.16
14.37
zoo Gms.
tt. Sol.
AgsS04.
1.023
1. 127
1.247
1.340
I 450
1.524
Results at 75*.
Gms. per 100 Gms.
Sat. Sol.
Results
Gms. Der
K«S04.
3.12
5-73
8.43
10.55
13.17
17.06
AASO4.
1.273
1.406
1.554
1.665
1.806
2.02Z
3.23
5.60
8.45
11.30
15 07
18.58
at 100^.
zoo Gms.
Sol.
Ag|S0«.
1.488
1.675
1.890
2. 115
2.410
2.677
Results at 14.5^ are also givea
Solubility of Silver Sulfate in Aqueous Sodium Sulfate Solutions.
Results at 33''.
Gms. per zoo Gms.
Sat. Sol.
NaiS0«. * AgjSO*.
0.25 0.861
0.98 0.816
2.01 0.832
3 0.867
5.34 0.972
10.05 1. 150
20.09 1.448
29.55 I 570
39.44 1.462
46.976 0.932
Results at 14.5''
(Barre,
Results at 5I^
Gms. per zoo Gms.
Sat. Sol.
Ka«S04. Ag|S0«:
0.25 1.032
1.02 0.995
1.90 I. 017
2.92 1.053
5.40 I. 173
10. II 1.379
20.25 1.705
29.23 1.802
39.30 1.540
44.46 0.882
and at 18° are also
Z9ZO, Z9ZZ.)
Results at 75*.
Gms. Der zoo Gms.
Sat. Sol.
Na,S04. AgtSO;.
0.20 I. 215
0.98 I. 210
I . 96 I . 238
2 . 98 I . 296
5.37 1.458
9.81 1.697
19.98 2.075
29.66 2.138
38.94 1.603
41.36 I. 156
given.
Results at Ioo^
Gms. per zoo Gms.
Sat. Sol.
NaiS04. Ag^4.
0.50 I. 341
1. 01 1.363
I . 94 I . 418
3.02 1.494
5.33 1.651
10.15 2.012
25.45 2.351
34.72 2.012
38.63 1.687
40.16 I. 158
Solubility in Silver Sulfate in Aqueous 0.5 n Solutions of Various
Compounds at 25**.
(Rothmund, z9zo.)
Aq. 0.5 n
Solution of:
Methyl Alcohol
Ethyl Alcohol
Propyl Alcohol
Amyl Ale. (tert
Acetone
Ether
Formaldehyde
Glycol
Gms.
Dissolved
p^Xiter.
7.764
7.109
6.798
.) 6.36
6.86
6.424
7.078
8.076
Aq. 0.5 n
Solution of:
Gms.
Disserved
p^Liter.
8.202
Glycerol
Mannitol 9.262
Grape Sugar 8.418
Urea 9 448
Dimethylpyrone 6.736
Urethan 7. 078
Formamide 8.42
Acetamide 7*794
Aq. 0.5 n
Solution of:
Acetonitrile
Glycocol
Acetic Add
Phenol
Chloral
Methylal
Methyl Acetate
Gms.
Dissolved
per Liter.
16.37
13.50
7 857
II. 81
7.266
6.393
6.61
Fusion-point data for Ag^SOi + NasSOi are given by Nacken (1907).
8ILVBB SULnDE 624
SILVER SULnDE AgtS.
One liter H|0 dissolves about 4.ior~u gm, atoms Ag as sulfide at about 18".'
(Bemfeld. 1898.)
One liter HtO dissolves o.55.ior* gm. mols. ^^ 0.0001363 gm. AgiS at 18^.
(Weigd, 1907.)
Fusion-point data for AgiS -4- ZnS are given by Friedrich (1908).
SILVER 0X7LFONATES
SOLUBILITT IN WATER AT 20^
(Sandquiat, 19x2.),
Sulfan&t«. ^5*°»* Sulfonate"
bttUonate. p^ ^^ ^^ g^
Silver .2 Phenanthrene Monosulfonate] 0.099
.3 o . 20
" .10 " " 0.52
SILVER TARTRATE C4H«0«Agk.
100 gms. HtO dissolve 0.2012 gm. C«H40tAgk at i8^ and 0.2031 gm. at 25^
(Parthol and Hilbner, 1903.)
SILVER TmOCYANATE AgSCN.
:
Solubility in
Water.
f.
Gm. AgSCN per Liter.
Authority.
20
0.00014
(BOttger, 1903.)
21
0.00025
(Whitby, Z9IO. See'Note, p. 608.)
25
0.00017
(KOster and Thid, 1903.)
25
0.0002
(Abegg and Cos, 1903.)
100
0.0064
(B^tgec, 1906.)
Additional data for the solubility of AgSCN in water are given by Kirschner
(1912.)
Solubility of Silver Thiocyanate in Aqueous Potassium Thiocyanatb
AT 25*^. (Hellwig, 1900.)
Mob. KSCN
per Liter.
0.573
0.626
1.066
One liter of aqueous 3 n AgNOi dissolves 0.0432 gm. AgSCN at 25.2^ (Hellwig, 1900.)
SILVER VALERATES AgCiHtOi.
Normal Valerate, CH,(CH,),.COOAg. Iso Valerate, CH,.CH(CH,),CHiCOOAg.
Solubility of Each Separately in Water.
(Forth, z888; Sedlitzky, 1887.)
Gms. per 100 Gms. HjO.
Mob. A^SCN
per lAter.
0.0124
0.0168
Gms. A^(3f
perLner.
2.06
2.08
Mob. KSCN
per Liter.
1. 12
i.20
Mob. AjsSCN
per Liter.
0.0975
0.120
Gms. A^CN
per Liter.
16.18
1993
0.0850
14.01
125
0.134
22.34
»•.
Normal V.
isov:
0
0.229
0.177
10
0.259
0.211
30
0.300
0.246
30
0349
0.283
40
0.408
0.321
Cms. per xoo
Gms. HsO.
* • Normal V.
SO 0474
60 0552
70 0.636
80
lte at 20^
IsoV.
0360
0.401
0443
0.486
(Markwald, 1899.)
ICG gms. HiO dissolve 0.73 gm. silver valerate at 20 .
100 oc. sat. aq. solution contains 0.71 gm. dextro silver valerate at I5^
CI^vemBi 1900^)
635
SILVER VALERATE
SoLUBiLrrY OF Silver Valerate in Aqueous Solutions of Silver
Acetate, Silver Nitrate and of Sodium Valerate.
(Arrhenius, 1893.)
In Silver Acetate at 17.8'
[Mob, per Liter.
CiHAAg.
O
0.0067
0.0135
0.0270
0.0505
CfcHAAg.
0.0094
0.0070
0.0057
0.0037
0.00265
Gms. per Liter.
CsHAAg. COIAAg.
O
1. 13
2.27
4.54
8.48
1.96
1.46
1. 19
0.77
0.55
In Silver Nitrate at 16.5*.
Mols. per Liter. Gms. per Liter.
AgNO,. CtHAAg.
AgNOk.
O
0.0067
0.0133
0.0267
O.IOOO
CHAAg.
0.0094
0.0068
0.0051
0.0031
0.0012
O
1. 14
2.29
4.58
CiHANa.
O
0.0175
0.0349
0.0698
o. 1395
In Sodium Valerate at i8.6^
Mols. per liter. Gms. per Liter.
CAOsNa.
COIiQiAg.
0.0095
0.0047
0.0030
0.0018
0.0015
O
2.17
4.32
8.65
17.31
CiHtO^Ag.
1.986
0.982
0.627
0.376
0.313
1.96
1.42
1.07
0.65
0.25
SILVER VANADATE AgeVA,.
One liter of aqueous solution contains 0.047 gm. at 14^ and 0.073
SODIUM Na.
Solubility in Liquid Ammonia.
(Ruff and Geisel, 1906.)
em. at 100^
(Canelly, 1873.)
r.
-105
- 70
- so
Mob. NH| Required
to Dissolve i Gm.
Atom Na.
4.98
5.20
S-39
Mols. NH« Required
t*. to Dissolve z Gm.
Atom Na.
-30 5 52
o 5.87
+22 6.14
Solubility of Sodium in Melted Sodium Hydroxide.
(von Hevesy, 1909.)
Gms. Na per 100 Gms. NaOH 25.3
600^
10. 1
610**
9-9
670°
95
760^
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.
Thallium
((
a
Gms. Added Gms. Dissolved
Metal per zoo Na per zoo
Gms. NaOH.
S-40
8.30
12.42
31-37
Gms. Solvent.
23.13
23. 54
21.29
20.91
Added
Metal.
Cadmium
Gold
tt
Zinc
Gms. Added
Metal per zoo
Gms. NaOH.
2.87
3.16
6.03
8.22
30.37
Gms. Dissolved
Na per zoo
Gms. Solvent.
24.34
24.29
23.92
23.39
25.38
SODAMMONIXJM Nat(NHs)i.
100 gms. liquid ammonia dissolve 60.5 gms. Nat(NHs)i at —23^ 56.4 gms. at
o^, 56 gms. at +5^ and 55 gms. at 9^ Qoannis, Z906O
SODIUM ACETATE
626
SODIUM ACETATE CHiCOONa.3HiO.
Solubility in Water.
(Green, 1908.)
r.
Gms.
CHaCOONa
per zoo
Gms. H^.
SoUd Phase.
f.
(jfllS.
CH,CX)ONa
per 100
Gms. H^.
— 10
-18
19
30.4
Ice
20
30
"3.5
126
— 10
33
CHtCOONa
.3H/)
40
129.5
0
+10
20
36.3
40.8
46.5
u
so
60
70
134
139 -5
146
30
40
54-5
65- 5
tt
it
80
90
153
161
50
S8
83
138
tt
tt
100
no
170
180
0
119
CHtCOONa (unstable)
120
191
10
121
It
(C
123 b. pt.
193
Solid
CH,CXX>Na (imrtabl^
«
M
M
U
U
M
M
' Results differing somewhat from the above are given by KOhler (1897) ; Enldaar
(1901) and Schiavor (1902).
Solubility of Sodium Acetate in Aqueous Solutions of Acetic Acid at
Various Temperatures.
(Dunningham, 19x2.)
Results at o". Results at 15"*. Results at 30". Results at 75^
Gms. per zoo Gms.
Sat. Solution.
NaaO. (CH,C0)A
Gms. per zoo Gms.
Sat. Solution.
Na^O. (CH,C0),0.
29.34 O.IS
Gms. per 100 Gms. Gms. per zoo Gms. Solid Phase
Sat. Solution. Sat. Solution.
m
NaiO. (CH,CO),0'. NaiO. (CH,C0)A E«ch Case.
76 CH«C00Na
24.12 2.04
14.46 8.55
9.72 31
9.77 41.23
9.04 43.94
25.94
15-49
"45
11.25
10 -33
10.22
4.19
12.01
23.54
34.56
39.08
39-73
9.16 4932
35.31 0.77
26.25 8.92
• • • • • ■
25.98 9.06
18.09 13.62
13.53 21.88
13.24 33.05
13.14 32.90
7.64 65.07
44
32
22
17
II
7
o
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
1.02
0.79
54.34
61.63
70.55
77.60
86.61
95.87
98.09
7.67
7.33
6.61
5-52
3.78
2.94
1.27
66.42
69.68
72.85
77.76
83-92
86.73
94.78
45
47
30
o
5
36
85
05
63
44
43
65
81
98
03
69
•<
tt
CH|C(X)Na.3H^
tt
tt
tt
+X.I
06
X.X
71
M
49
M
35
M
•
«
•
X.t
M
+w
I.I = CH,C(X)Na.CH,COOH. 1.2 = CH,COONa.2CH,COOH.
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 (1911-12).
One determination at 25**, expressed in terms of volume of solution, is given by
Herz (1911-12). Two determinations at lO** similarly expressed, are given by
Enklaar (1901).
Data for the freezing-point of mixtures of sodium acetate and acetic add are
given by Vasilev (1909).
627
SODIUM ACETATE
Solubility of Sodium Acbtatb in Aqueous Ethyl Alcohol at 25^
(SddeU,
1910.)
Wt. Per cent
Q^Hin
Solvent.
O
ID
20
30
40
50
(2m of
Sat. Sol.
Gma. CH«COO-
Na.3H^ per loo
Gms. Sat. SoL
1.209 557
I. 160 S3
1.13s 49.8
1. 108 46.5
1.072 42
1.038 37
The solid phase in contact with the solution was CHiCOONa.sHtO in all
cases.
100 gms. absolute alcohol dissolve 7.49 gms. CHtCOONa.3HsO at room temp.
(BCdtker, 1897.)
Solubility of Sodium Acbtatb in Aqueous Alcohol:
Wt. Per cent
aiLOHin
Solvent.
4m of
Sat.SQL
Gms.CHtC00-
Na.3H^ per zoo
Gms. Sat. SoL
60
0.990
30.4
70
80
0.942
0.882
22.8
13
90
95
0.838
0.828
6.7
6.1
100
0.823
7.3
At 1 8*.
(Gerardin, 1865.)
Wt. Gms. CHaCOONa
Per cent per 100 Gms.
Alcohol. Aq. AkohoL
38
35-9
At Different Temperatures.
(Schiavor, 1902.)
5-2
9.8
23
29
38
45
59
86
91
29.8
27.5
23.5
20.4
14.6
3.9
2.1
f.
8
12
19
II
13
15
18
21
23
Degree
Akohol.
98.4
98.4
98.4
90
90
63
63
63
40
Gms. per zoo Gms. Alcohol.
CH«C00Na. CH«C00Na.3H«0.
2.08
2.12
2.33
2.07
2.13
13 46
13.88
14.65
28.50
3.45
3.51
3.86
3.42
3.52
22.32
23.03
24.30
47.27
100 gms. H|0 dissolve 237.6 gms. sugar + 57-3 gms. CHiCOONa, or 100
gms. of the saturated solution contain 58.93 gms. sugar + 14*44 gms. CHiCOONa
at 3 1 .25^ (KOhler, Z897.)
100 cc. anhydrous hydrazine dissolve 6 gms. sodium acetate at room temp.
(Welsh and Broderson, 19x5.)
100 gms. propyl alcohol dissolve 0.97 gm. sodium acetate. (Schlamp. Z894.)
SODIUM SulfoANTIMONATE Na,SbS4.9HiO.
Solubility in Wateb.
(Donk, Z908.)
Gms.
Gms.
Gms.
f.
Na|SbS«per
Solid
f Na,SbS« per SoUd
" * zoo Gms. Phase.
r.
Na,SbS« per Solid
100 Gms.
Phase.
zoo Gms. Phase.
Sat. SoL
Sat. Sol.
Sat. Sol.
—O.I
0.5
Ice
— 1.75 II. 2 Ice
49-6
38.9 Na.SbS4.9H/>
—0.65
4
<i
0 1 1. 8 Na«SbS«.9H^
59.6
45
-0.9
5.7
<(
15 19.3
69.6
50.7
— 1.26
7.8
M
30 27.1
79.5
57.1
-1.45
9.2
It
38 32
^
Solubility of Sodium Sulfoantimonate in Aqueous Solutions of Sodium
Hydroxide at 30®.
(Donk. Z908.)
Gms. per zoo Gms. Sat. SoL « ,,^ «^ Gms. per zoo Gms. Sat. Sol. „ „ . ^,
Na«SbS«.
NaOH.
> ooua jrnase.
'Na,SbS«.
NaOH.
i aoua jrnase.
27.1
0
Na,SbS4.9H/>
16.4
42.6
NasSbS4.9Hd0
13
9.9
M
17.7
47.2
"+NaOH.H,0
5-9
24.8
M
9.1
49.5
Na0H.H«0
10.5
32.9
M
0
54.3
SODIUM SuUoANTIM ONATE
628
Solubility of Sodium Sulfoantimonatb in Aqueous Solutions of Sodium
Thiosulfatb.
(Dook, 1908.)
Results at o^
Results at
30-.
Cms. per 100 Gim. Sat. Sol.
Gms. per zoo
Na.SbS«.
Gms. Sat. Sol.
NaAQi.
Solid Phase.
'N^SbS,. N.,SA. Solid Phue.
II. 8 0 Na«SbS|.9H/>
19.9
7.7
NaiSbS|.9B^
4.4 4.9
"•5
16.4
<i
0.8 14.6
4.2
37.7
«
o.i 27.3 •*
I
43.8
M
0 33.6 «+N«AOb.sH^
I
47
It
0 33.6 Na.SA.5HiO
I
47.8
" +NaA0b.sHi0
0
45.8
NatSA-sHiO
Solubility of Sodium Sulfoantimunatb in Aqueous Ethyl Alcohol.
(Dook, X908.)
Results at o^.
Gms. per 100 Gms. Sat. Sol.
Results at 30^
Gms. pet 100 Gms. Sat. Sol.
Results at 65^
Gms. per 100 Gms. Sat. SoL
Na.SbS«. CtH»OH. Na«SbS«.
CAOH.
Ka,SbS«. CAOH.
II. 8 0 19.3
s
47.9 0
8.2 3.7 14.6
3.2 12.7 6.4
0.9 29 1.2
0 60.8 0
10.3
24.8
46
76.2
39.3 4.7
36. 5 8*
4.1 54. I*
0 81
* Two liquid layers separate between these conoentimtioos of alcohol.
these coQJoiiied utyeis is as follows:
The oomposttioa of sevei
Gms. per zoo Gms. Alcoholic Layer.
Gms. per zoo G
Na«SbS«.
36. 5
ms. Aqueous Layer.
' Na«SbS4. CH»OH.
4.1 54.1
r,H,0H. '
8
10.2 40.4
14. I 33 5
0
27.8
24.1
18
14.3
18.8
27.2
The solid phase in contact with each of the above solutions is Na<SbS«.9H^.
Solubility of Sodium Sulfoantimonatb in Aqueous Methyl Alcohol.
(Donk, X908.)
Results at o^.
Gms. per zoo Gms. Sat. Sol.
Na«SbS|.
8.6
2.8
2.1
0.3
0.1
0.05
0.2
2
CH^H.
3-4
15.5
23.1
50- 3
57
81.7
92
95.9
SoUd Phase.
Na«SbS«.9H^
u
M
M
M
Results at 30^.
Gms. per zoo Gms. Sat. Sol.
Na,SbS«.
27.1
12.8
5.8
0.1
0.1
1.2
3.9
CH^H.
O
18. 1
33.1
65.7
84.2
91.2
94
SoUd Phase.
Na«SbS|.9Hd0
u
M
M
m
SODIUM ABBENATK Na.As04.i2H|0.
100 gms. aqueous solution contain 21. 1 gms. NasAs04.i2H|0 (« 10.4 gms.
NasAsOi) at 17**. Sp. Gr. of solution => 1.1186. (Schi£F. z86o.)
100 gms. glycerol dissolve 50 gms. sodium arsenate at 15.5^. (Osseodowskl, 1907.)
629
SODIUM ABBENATKS
Equilibrium in the System Sodium Oxide, Arsenic Trioxidb, Water at 25*
(Schidnemaken and de Baat, igz?-)
Gms. per xoo Gma. Sat. Sol.
A3A.
NaaO.
Solid Phase.
AsA.
Na^.
-% Solid Phaie.
2.019
0
AsA
31-05
21.82
Na4A3rf)4.9lV>
14. 45
2.45
u
lfc29
lfc22.7
" +Na»A««Ou.26H^
24.42
4- 23
u
21.92
24.04
Na»Aa«Ou.26HiO
37.73
6.46
((
17.50
25.64
It
58.54
9.60
tt
14.26
29.16
M
±73
d=I2
" +NaA80b
14.63
30.24
(1
63.01
12.73
NaAsQi
19.32
32.04
«+Na4AaA
57.90
13.24
tt
15.53
33.57
Na^AaA
48.05
14.27
tt
10.49
36.21
tt
36.32
18.74
u
6.59
39.39
" +NaOH.H^
±34
±21.1
" +Na4AaA.9HiO
5."
39 69
NaOHJO^
32.24
21.6
Na4A9A.9H/)
0
41.2
II
SODIUM Hydrogen ABBENATK NaiHAs04.i2HiO.
Solubility in Water.
(Average curve from results of Srhiff, i860; Tilden, 1884; Greenish and Smith, 190Z.)
X. Gms. NatHAsOi
per xoo Cms. H«0.
o 7.3
10 15.5
15 20.5(^-1.1765)
SODIUM Diethyl BABBrrUKATK Na(CsHnOsNs).
Solubility in Water.
(Puckner and Hilpert, 1909.)
f.
Gms. NasHAsOa
per zoo Gms. HgO.
f.
Gms. NatHAsOi
per 100 Gms. H/)
20
26.5
40
47
25
33
60
65
30
37
80
85
Gms. Salt per 100 Gms. Sat. Sol.
5'
6.08
15**
16.87
25"
17.18
91"
32.50
SODIUM BENZOATK CsH|CCX)Na.
Solubility in Aqueous Ethyl Alcohol at 25*
(Seidell, 1910.)
Wt. Per cent
qH.OH in
Solvent.
dnol
Sat. Sol.
Gms. CACOONa
per 100 Gms.
Sat. SoL
Wt. Per cent
QH.OH in
Solvent. ,
d»ot
Sat. SoL
Gms. CACOONa
per 100 Gms.
i Sat. Sd.
0
I -155
36
60
0.975
21.3
10
1. 132
35.3
70
0.927
15. 4
20
I.IIO
33.7
80
0.877
8.8
30
1.086
31.5
90
0.831
2.8
40
1.055
28.9
95
0.812
1.3
50
1.020
25.6
100
0.795
0.6
SODIUM (Tetra) BORATE NatBtOr.ioHtO (Borax).
Solubility in Water.
(Horn and Van Wagener, 1903.)
f.
Gms. NsfBA
per 100 Gms.
f.
Gms. N&|B|0|
per 100 Gms.
f.
Gms. Na|BA
per 100 Gms.
*
H,0.
H,0.
Hfi.
0.5
1-3
50
10.5
60
19.4
20.3
10
1.6
54
13.3
62
22
20.7
21.5
2.8
55
14.2
65
22
21.9
30
3.9
56
15
70
24.4
37.5
5.6
57
16
80
31.5
45
8.1
90
XOO
41
52.5
Tr. temp., NatB407.ioHtO-»NatB407.5HtO, approximately 62^
^16.6« of sat. sol. = 1.020. (Greenish and Smith. 1901.)
100 gms. H<0 dissolve 3.33 gms. NasB407 at 25", determined by refractometer.
(Osaka, 1903-08O
SODIUM BORATES
630
Solubility of Sodium Borates in Water at 30^.
(Dukdski, 1906, complete references given.)
Gms. per xoo
Gms. Solution.
Gms. per xoo
Gms. Residue.
Solid Phase.
NaaO.
BA-
Na^O.
BA. ^
42.0
• • •
■ • •
• • •
NaOH.H|0
41 -37
5.10
43
•54
4.19
M
38-85
sss
37
30
II. 18
Nas03iO»w|HaO
34-44
3-73
33
52
10.80
M
29-39
251
29
63
10. II
M
26.13
2-75
27
85
15.21
m
23.00
3 82
24.
91
11.60
<•
16.61
13.69
21.
29
20.64
M
21.58
4 63
24.
52
19 04
NasO^iOs^HflO +iNasO.B«Os.8H^
20.58
4.69
21.
61
16.59
Nas03sQi.8HsO
15-32
6.21
19
70
17.84
M
"39
9.12
18.
OS
18.17
M
8.85
10.49
II.
72
20.62
Na30.aBsQi.ioH^
5 81
6.94
10
8a
21.31
u
1.88
2.41
7
31
15-50
M
1.38
5.16
7
.i6
17.44
M
2.02
7-79
6
24
16.38
•<
4.08
17.20
8
.96
29.20
NaiO .aBsOft-xoHsO + NaaO-sBsO^oHjO
3-79
15.84
5
.68
28.19
NaaO-sBsOnoHaO
2.26
12.14
5
21
29.19
u
1.99
11.84
5
•74
39.66
NaaCaBsOs-ioHaO + B(OH)t
1.86
II. 18
I
.06
28.78
B(OH),
0.64
6. II
0
31
31 19
u
• • •
^'Kd
•
> •
• • •
M
Equilibrium in the System Sodium Oxide, Boric Oxide, Water at 60^.
(Sboigi and Mecacci, 19x5, 19x6.)
Gms. per xoo Gms.
Gms. per
Sat.
xoo Gms.
Sat.
Sol.
SoUd Phase.
Sol.
Solid Phase.
NaiO.
B,0,.
'Na«0.
BA.
49.25
0
Na0H.H|0
19.29
22.78
Na^.BA.4H^
48.44
0.81
It
20.30
25.50
ff
49.28
1-53
" -H2Na,0.BA.Hrf)
22.21
32.17
" +Na40.2BA.5HdO
47.38
2.24
3Na40.6.0,.Ha0
19.43
27.09
Na^.2BA.5HyO
44.74
3.78
««
16.13
23.05
ft
42.94
S.67
« +Narf).BA.IV>
13.51
19.10
ft
40.14
5-41
Na^.6.0,.HiO
11.58
16.62
u
38.70
S.56
i<
6.95
11.50
u
35-76
6.29
IC
5.65
14.89
u
34.93
6.80
Cf
6.84
20.40
t(
31.88
9.85
" (unstable)
8.42
28.05
it
29.56
11.83
« «
11.29
41.47
** +Na^.sBA.ioH^
28.07
14.65
If ft
8.29
33.57
NaaO.5BA.10H/>
33.12
7-47
" +Na^.BA.4H,0
6.29
28.77
ti
28.64
6.51
Na/).BA-4HiO
3.22
21.94
tt
22.06
10.29
ft
340
22.59
" +H,BQ|
18.72
17-33
fi
1.39
13.92
H,BQ,
18.32
19-17
«f
0
7.39
ft
SODIDM BORATES
631
«
it
It
tt
Solubility of Sodium Borates in Several Solvents.
Borate. Solvent. f. ,jSS'^3^,?St. Authority.
Sodium borate Alcohol (^=0.941) 15. 5 2.48 (u. s. p. vm.)
Glycerol 15.5 60.3 (U.S. p.vm.)
" 80 100 (U.S. p.vm.)
Sodium Biboiate Trichlorethylene 15 o. 011 (Wester and Bruins, 1914.)
Fusion-point data for mixtures of NaBOi+NaPOi and NaBOi+NaiSiOi arc
EVen by Van Klooster (1910-11). Results for NaiB4C)7+Na4P^ are given by
i Chatelier (1894).
SODIUM BBOMATB NaBrOs. *
Solubility in Water.
(Kremers, iSss-sSa.)
t''. O"" 20** 40*^ 60** 80'' 100**
Gms. NaBrOs per 100 Gms. H^ 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. NaBrOi with decomposition.
(Welsh and Broderson, 19x5.)
SODIUM BROMIDE NaBr.2H,0.
Solubility in Water.
f.
— 10. 1
-28
-23.5
— 20
— 10
o
+16.V
20
30
40
(z) Rudorff (1862); (2) Guthrie (1875): (3) Panfiloff (1893); (4) de Coppet (1883); (5) Richardi
and Churchill (1899); (6) Etard (1894); (7) Cocheret (1911); (8) Greenish (1900).
Gms. NaBr per
xoo Gms. Sat. Sol.
SoUd Phase.
f.
Gms. NaBr per
zoo Gms. Sat. Sol.
Solid Phase.
20.8 (l)
Ice
■ 50
53.7(4)
NaBr.3H/>
40.3 (2)
" +NaBr.sHie,
50. 7
53.9(5)
" +NaBr
41 . 2 (3)
NaBr.sH,0+NaBr.a
HdO
80
54. 2 (4)
NaBr
41.8(4)
NaBr.sH/)
100
54.8(4)
42.9 (4)
i<
no
55.1(4)
44-3 (4)
M
140
56.5(6)
47 (8)*
M
180
59.5(6)
47.5(4)
M
210
60.9(6)
49.4(7)
«
230
62 (6)
51.4(4)
1.523).
Solubility of Sodium Bromide in Aqueous Solutions of Sodium
Hydroxide at 17®.
(Ditte, Z897.)
Gms. per zoo Gms. HjO. Gms. per zoo Gms. H3O.
Gbs. per zoo Gms. H^.
>JaOH.
NaBr:
KaOH.
NaBr:
KaOH.
NaBr.
0
.0
91
•38
17.17
63.06
28.43
48.00
3
.26
79
.86
19.12
62.51
36.61
38.41
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, Z9zz.)
Gms. per zoo Gms. Sat. Sol.
CiHiOH.
O
11.79
31.78
43.22
54.59
NaBr.
49-4
42.9
32.12
26.79
20.83
Solid Phase.
NaBr.2H^
«<
II
•I
Gms. per zoo Gms. Sat. SoL
CHiOH.
NaBr. '
ooiia x'aoac.
65.51
16.08
NaBr.2H/)
72.36
13.41
11
76.92
12.03
" +NaBr
87.35
7.44
NaBr
97.08
3.01
cc
SODIUM BROMIDE
632
Solubility of Sodium Bromide* in Alcoholic Solutions.
(RoUand, 1898^5; de Bniyiit 1892; Eder, 1876.)
Alcohol.
Conomtratioo
of Aq. Alcohol.
f.
ums. najsr
per 100 Gma.
Alcohol.
Methyl Alcohol
^w= 0.799
room temp.
21.7 (R.)
Ethyl
rfn=o.8io
«
7.14
Propyl
rfn=« 0.816
((
2.01
Ethyl
90% by vol.
?
4.0 (hydnted NaBr)
Methyl
Absolute
19 s
17.35 (<fcBrayn)
Ethyl
C(
IS
6.3 (NaBraHsO) (Eds^
Ethyl Ether
•f
IS
0.08
^ A sat. solution of NaBr in CHiOH contains 0.9 gm. NaBr per 100 gms. solu-
tion at the critical temperature. (Ccntnerazwer, 1910.)
100 cc. of ethyl alcohol of d ^ 0.8327 dissolve 7.37 gms. NaBr at 16.4^, dit of
sat. sol. B 0.889. (Greenish, 1900.)
100 gms. propyl alcohol dissolve 2.05 gms. NaBr at ord. temp. (SchUmp, 1894)
S(H.uBiLiTY OP Sodium Bromide in Mixtures of Alcohols at 25®.
(Hen and Kuhn, 1908).
Sat. Sol.
In CHjOH -f C,H*OH.
Per cent
CH^H
in
Mixture.
o 0.8189
4.37 0.8265
10.4 0.8273
41.02 0.8593
80.69 0.9079
84.77 0.9104
91.25 0.9235
roo 0.9238
In CHiOH + CiHtOH. In CiH»OH + C1H7OH.
Gms.
NaBr per
100 cc.
Sat. Sol.
2.93
3.65
4.04
7.24
12.51
12.86
14.32
14.40
Per cent
CbHtOH
in
Mixture.
O
II. II
23.8
65.2
91.8
93.75
100
4a of
Sat. Sol.
0.9238
0.9048
0.8887
0.8390
0.8153
0.8144
0.8093
Gms.
NaBr per
100 cc.
Sat. Sol.
14.40
12.43
10.53
4.42
1.47
1.26
0.74
Percent
C1H7OH
in
Mixture.
O
8.1
17.85
56.6
88.6
91.2
95-2
100
d% of
Sat. Sol.
0.8189
0.8147
0.8145
0.8107
O.8116
0.8083
0.8090
0.8093
Cvms.
NaBr pa
100 cc.
Sat. Sol.
2.93
2.49
2.47
1.90
I. II
0.83
0.82
0.74
Solubility of Sodium Bromide in Acetamide at Various Temperatures.
(Menichutkin, 1908.)
Gms. per xoo Gms.
oat. Sol.
NaBr.2CHi-_ T^j.p,
CONH, -NaBr.
f.
82*
86
78
76
74
72
7ot
80
Gms. per xoo Gtoa.
Sat. Sol.
NaBr.aCli- . NaBr
CONH, ■ "*"'•
Solid Phase.
SoUd Phase.
6
".5
16.3
20.2
23
25
27
2.8
5.36
7.6
9-4
10.7
II. 6
12.6
CHaCONHi
•-HNaBr.2CH,C0NH,
NaBr.3CH,C0NH,
90
100
1 10
120
130
i3St
iSS
175
29.4 13.7 NaBr.aCHtCONHi
32.2 15
35-3 16.4
38.7 18
42.6 19.8
45-3 21. I
46.4 21.6
47.5 22.1
+NaBr
NaBr
It
• M.pt.
t Tr. pt.
t Eutec.
100 gms. 95% formic acid dissolve 22.3 gms. NaBr at 18.5®.
100 cc. anhydrous hydrazine dissolve 37 gms. NaBr at room temp.
(Welsh and Br
(Aschan, 19x3.)
troderson, x9x5.)
Fusion-point Data (Solubilities, see footnote, p. i) Are Given for the
Following Mixtures.
NaBr + NaCl
NaBr + Nal
NaBr + NaF.
NaBr + NaOH
NaBr + NaNOj.
NaBr + Na«SO#
(Amadori, 191 2a; Ru£F and Plato, 1903.)
(Amadori, 1912a.)
(Ruff and Plato, 1903.)
(Scarpa, 1915.)
(Meneghini, x9x2.)
(Ruff and Plato, X903.)
SODIUM CACODYLATB
633
SODIUM CACODYLATE (CHOtAsO.ONa.
loogms. HiO dissolve about 200 gms. of thesalt at i^°-20^ (Squire and Caines, 2905.)
loooc. 90% alcohol dissolve about loogms. of thesalt at 15^-20^ " **
SODIUM CAMPHORATIS
Solubility in Aqubous d Camphoric Acid Solutions at I3.5^-I6^
(Jongfldsch and Landrieu, 19x4.)
Gms. per xoo Gms.
Sat. Sol.
Gms. per xoo Gms.
Solid Phase. Sat.
Sol. Solid Phase.
CidHi^4. C»Hu0«Nat^
P»HiA.
C»Hu04Na;.
0.621 0 CioHiA '2.87
25.62 CMHtfO4Na.2C10HtfO4.sHdO
2.03 .4.19
2.89
27.41 "
2.87 8.32
2.74
30.69
3.03 10.05
2.63
32.75
2 . 97 7 . 80
" +CioHu04Na.2CioHi/)«.2H^ 2.29
40. 10 CMHuO«Na.H^ (or IH^C^
2.87 9.06
C]DH]ip4Na.sCMHi/)4.3H^ 2 . 1 7
40.54
2.94 10.46
1.06
47.04
2.68 14.99
0.88
49 . 60 CMHu04Nat.3H^
2.64 17.53
0
50. 2
C10H16O4 = Camphoric acid. C10H1sO4Na.2C10Hi6O4.2H1O" Monosodiumdtri-
camp>horate. CioHi«04Na.HtO = Mono8odium d camphorate. CioHi404Nai.3HsO
» 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 17^-23° are also given.)
SODIUM CABBONATB NaiCOtioHsO.
Solubility in Water.
(Weils and McAdam, Jr., 1907; Mulder, below 27* and above 44*.)
Gms.
Gms.
f.
N8«CQ| per
100 Gms. afi.
SoUd Phase.
f.
NstCQi mr
xoo Gms. H|0.
Solid Phase.
0
7
N8t(X),.xoH^
34.76
48.98
N8tC0k.7H^
5
9.5
II
35.62
50.08
II
10
12.5
M
35.50
• • •
" +Na,CQ,.Hi0
IS
16.4
II
29.86
50.53
NatC0i.H^
20
21. 5
1*
31.80
50.31
II
27.84
34.20
l«
35.17
49.63
II
29.33
37.40
II
36.45
49.36
a
30.35
40.12
II
37.91
49.11
M
31.45
43.25
11
41.94
48.51
M
32.06
45.64
II
43-94
47.98
u
32.15
• • •
" +Na«C0|.7H^
60
46.4
M
33.10
■ • •
" +Na«C0|.Hd0
80
45.8
€»■
30.35
43.50 -
NatC0t.7Hi0
100
45. 5
M
32.86
46.28
•I
105
45.2
M
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 Ldwel, 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 (191 1) and Cocheret
(1911).
Sp. Gr. of solution saturated at 17.5", 1.165 (Hager); at 18", 1.172 (Kohl-
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
Equilibriuii in the System Sodium Carbonate, Sodium Bicarbonate,
AND Water at 35°.
(McCoy and Test, 191 1.)
T(Forty grams of NaHCC^ and about 200 cc. of H|0 were rotated at 25" until
equilibnum 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 NatCOi.ioHsO were then added,
and the mixture again rotated until equilibrium was reached, and again analyzed.
This was continued and the following results were obtained.)
Per cent of
Total Na
Present as
Bicarbonate.
O
S-92
7-5
10
12.89
IS
20
32
S6
80
100
Gms-Na
per Liter.
119. 9
127.6
120
107
108
100
80
60
40
30
27.02
Gms.
Bicarbonate
per Liter.
O
27.6
Gnas. Carbonate
per Liter.
SO
98
8
276.4
276.3
316.6
Solid
Na«C0k.xoH/)
** +NatCOk.NaHCO».aH/>
NatCQ|.NaHCQ|.2H^
* " +NaHC0,
NaHCQi
M
M
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 (191 1).
Gms. per lOo Gms. H^D
KatCOt. '
28.3
273
26.5
19.2
NaHCOa.
O
2.1
4.2
S-7
Solid Phase.
NatCQ|.ioH^
Gms. per 100 Gms. H|0.
KatCO,. ^
M
" +NaHC0k
NaHCOk
12.4
6.2
I
NaHCOi.
7.3
9
10. 1
Solid Phase.
NaHCOb
Solubility of Sodium Carbonate in Aqueous Solutions of Sodium
Bromide and of Sodium Iodide at 30^
(Cochent, xQxz.)
In Aq. NaBr Solutions.
[n Aq. Nal Solutions.
Gms. per xoo Gms. Sat. Sol.
Solid PhaM
Gms. per xoo Gms. Sat. Sol.
Solid Phase.
Na«CQ,.
NaBr.
OUUU f USaC.
'NatCQ,.
Nal.
27.98
0
Na«CO|.ioII|0
26.5
2.4
NatCQ|.zdHiO
27 54
2.41
i<
255
4.7
tt
26.72
4.06
11
24.4
8.6
u
26.23
6.26
" +Na.CQ,.7H/)
24.3
95
" +Na.C0>.7H/)
23.40
II
Na«CQ|.7Hi0
23
II. 2
Na«C0k.7H«0
22.68
12.22
M
20.8
14
<i
19.86
16.88
If
18.7
18.4
If
19.57
16.95
« +Na.C0>.Hd0
iS-3
25.4
" +NatC0^.Hd0
18. II
19.32
Na«CQ|.Hi0
13.1
29.1
Na,CO|.H/)
8.4S
33-39
M
10.4
33.3
ii
6.90
36.13
M
4.2
46
If
3 04
44.75
•1
2.7
.51
•1
2.99
45. 31
" +NaBr.aIV>
0.9
57.6
11
2.60
45.68
NaBr.aH^
0.3
65.6
" +NaI.aIV>
0
49.40
u
0
65.5
NaI.sH«0
u
M
M
635 SODIUM CABBONATK
Solubility of Sodium Carbonate in Aqubous Solutions of Sodium
Chloride at 15®.
(Reich, 1891.)
Cms. per TOO Gnu. Gms.NaCl Gms.Na,C0i Gms. pg 100 Gms. GnM-NaQ Gms-NauCQi
"<fJ- per per loo Gms. HiQ. per per loo Gms.
VT /-I NaiCX)i.io- 100 Gms. NaCl rTT. Na«C0>.xo-' too Gms. NaCl
NaCL ""^Jg;*^ Solutkm. Solution. NaCl. ""^^ ^ Solution. Solution.
O 61.42 o 16.42 23.70 3906 15.96 9.76
4.03 53.86 2.92 14.47 27.93 39-73 18.26 9.62
8.02 48 5.80 12.87 31-65 41.44 20.06 9.73
12.02 43.78 8.61 11.62 35.46 43.77 21.75 7.95
16.05 40.96 II. 31 10.70 37.23 45-27* 22.46 10.13
19.82 39.46 13.71 10. II
* Both aalU in solid phase.
Solubility of Sodium Carbonate in Aqueous Sodium Chloride at 3o".
(Cochexet, 19x1.)
Gms. per xoo Gms. Sat. Sol. , _ ,. . «, Gms. per xoo Gms. Sat. Sol. » ,. . ^.
^-— -^j • iTTT^ Solid Phase. ^ ^ \Z, ' XTT^ — » SoUd Phase.
NaiCOs. NaCl. Na|C0|. ^aCl. i
27.98 O NaaC0|.xoH^ 20.72 11-49 NaaC0|.H^
27.48 0.90 " 18 14.12 '' +Naa
27.12 3.33 " 14.81 16.26 NaO
26.82 4.15 " +NaaC0|.7H40 9.71 18.76
25-59 5-17 Na,C0«.7H^ 5-65 21.94
24.26 5.93 " o 26.47
22.75 10.24 " +NaaC0k.H^
Solubility of Sodium Carbonate in Aqueous Solutions of Sodium Nitrate.
(Kremann and Zitek, 1909.)
^ Gms. per xoo Gms. HjO. _ ... _. ., Gms. per xoo Gms. HjO. _ ... _.
t*. < * 0 > Solid Phase. t . « ^ -* Solid Phase.
NatCOi. NaNOk. ^u« i^"*- • - Na,CO,. NaNO,, ^"«^™«-
10 11.98 o NatCO^xoH^ 24.2 24.63 54-43 KatCO^-rH^
10 8.75 70-48 " +NaNO, 24.2 21.8 62.7 " +NaNOb
10 O 80.5 NaNOi 24.2 5.96 84.45 NaNOb
24.2 28.55 O NatCOk.xoH«0 24.2 O 91.3 "
24.2 26.33 45 96 " +Na,C0,.7H^
Solubility of Sodium Carbonate in Aqueous Ethyl Alcohol at 3o".
(Cocfaeret, x9xx.)
Gms. per xoo Gms. Sat. Sol. _ ,. , _. Gms. per 100 Gms. Sat. Sol. _ ... _,
'^ Sohd Phase. t * » Sohd Phase.
NajCO,. CHiOH. ^"ariaac. Na,CO,. CH,0H. ^^a ^"s*.
26.61 2.64 NatC0k.xoH^ 0.40 63.20 Na|C0k.7H^
26.14 3-41* " O.ll 73.06 " +Na«CQ|.H^
1.38 44.81* " 0.07 78.19 Na,C0k.H^
0.62 52.99 " 0.06 90.95
0.53 5570 " +Na,C0».7H,0 0.03 95.06 " -f Na,C0,
0.51 56.56 NaaC0|.7H^ ... 98.46 NatCO^
* Between these two concentrations, the mixtures separate into two liquid layers.
Results are also given for the solubility c^ NasCOt + NaBr and of NatCQi
+ NaCl in Aq. C,HjOH at 30*.
Solubility of Sodium Carbonate in Aqueous Solutions of Ethyl and of
Propyl Alcohol at 20". ,
(LinebaxiBr, X892.)
Wt. Per cent
Gms. NssCO
UESL
xoo Gms. Sol.
Wt. Per cent
Alot^L
Urns. NaiUJi p
er xoo ums. boi.
AlcohoL
In Ethyl.
In Propyl.
• InEthyL
InPropyL
28
• • •
4.4
48
0.9
1-3
38
■ • •
2-7
50
0.84
1.2
44
1.7
1.7
54
0.80
0.9
46
1. 13
1.5
62
• • •
0.4
SODIUM CARBONATE
636
Solubility of Sodium Carbonate in Aqueous Solutions of Etbttl Alcohol.
(Ketner, 1901-oa.)
Note. — The mixtures were 90 made that alcoholic and aqueous layers were
formed, and these were brought into equilibrium with the solid phase.
t*
Gms. per 100 Gms. Alcoholic Layer.
Gms. per
100 Gms. Aq. Layer.
A
Solid Phase.
w •
'^CH.OH.
Na,C0s.
H,0.
r,H,0H.
NotCQi.
H1O.
35
62.9
0.3
36.8
I
32.4
66.6
Nstccvn^
40
61
0.4
38.6
1.2
31-9
66.9
(4
49
61
0.4
38.6
1.2
31. 5
67.3
M
68
55.8
0.9
43.3
2.3
28.8
68.9
u
312
52.4-
0.8
46.8
• • •
29.3
• * •
Ns,C(V7Hi0(»
31.9
54-8
0.7
44.5
1.7
29.8
68.5
M
32.3
56.1
0.6
43-3
1.5
30.2
68.3
a
33.2
58.1
0.5
42.4
1.4
31
67.6
«
27.7
Crit. sol.
± 14% CjHjOH ±
i3%Na«CO,=b73%Hrf)
28.2
23- 5
7-3
69.2
7.9
18.6
73.5
NstCXVioHyO
29
32.7
3.8
63.5
4.3
22.7
73.0
a
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
tt
Solubility of NasCOi.ioHtO in Dilute Alcohcx^ at 21'
(Ketner.)
Gms. per xoo Gms. Solution.
Gms. per xoo Gms. Solution.
NajCOj.
CH»OH.
H,0.
18.5
0
81.5
12.7
6.2
81. 1
6.9
15.3
77.8
3-2
26.1
70.7
NsiCO,.
CAOH.
H^.^
1.2
39.2
59.6
0.2
58.2
41.6
O.I
67.1
32.8
0.06
73.3
26.64
Isotherms showing the compositions of the conjugated liquids at 28.2% 29-7^
and 40^ are also given.
EguiLiBiauM in the System Sodium Carbonate, Normal Propyl Alcohol
AND Water at 20**.
(Ftankforter and Temple, 19x5.)
(Note. In this paper the results for the binodal curve are reported in terms of
gms. per 100 gms. solvent (water + alcohol), instead of gms. per 100 gms. of the
homogeneous liquid (sodium carbonate + water + alcohol.)
Gms. per
xoo Gms. Alcohol + Water.
A
Gms. per
xoo Gms. Alcohol + Wlater.
Na,COj.
Alcohol.
Water.
NmCOi.
Alcohol.
Water.
16.568
3.409
96.591
1.990
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
II. 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 resiflts 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. NajCOj at i5"-i6".
(Oasendowski, X907.)
100 gms. saturated solution in glycol contain 3.28-3.4 gms. sodium carbonate.
(de Coninck, xgos.)
100 gms. HiO dissolve 229.2 gms. sugar + 24.4 gms. NajCOa, or 100 gms. sat.
aq. solution contain 64.73 gms. sugar + 6.89 gms. NasCOi at 31.25®. (Kfihler, 1897.)
637
SODroM GABBONATE
Equilibrium in the System Sodium Carbonate, Pyridine, Water.
(Limbosch. 1909.)
Very pure materials were used. The boiling-i^oint (cor.) of the pyridine was
115^-115.07^. 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. Durinjg^ 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.
Percent
of
NatCOt.
0.129
0.129
0.129
0.129
0.129
0.129
0.129
0.129
1. 01
1. 01
1. 01
1. 01
1. 01
1. 01
1. 01
1. 01
1. 01
1. 01
2.50
2.50
2.50
2.5^
2.50
2.50
Percent
of
Pyridine.
66.2
66.4
67.7
69.2
73. S
74.8
76.1
77.8
47.6
49.9
512
52.2
S6.i
60.6
66.8
75.1
76.9
78.1
36.3
37-9
39.2
40
43-6
47.6
r of Sat.
12
25
36
44
53
51.5
Percent
of
Na«CO|.
2.50
2.50
2.50
2.50
2.50
2.50
2S.s(-64) 3.49
" (-59) 3.49
17
36
55
72
107
III
no
86.5
22
53.25
74.5
94
147
185
3-49
3-49
3.49
3.49
3-49
3.49
5.23
5.23
5. 23
5. 23
5.23
5.23
5.23
5- 23
5.23
Percent
of
Pyridine.
50
53.3
59.4
69.2
73.8
74.8
30.3
32.6
34.3
36.7
37.4
42.5
69.6
71.2
23.3
23.7
24.6
26.2
28.7
32.5
36.6
37.2
55-4
r of Sat.
199
197
173
123
no
6.12
6.12
6.99
6.99
• 6.99
—0.5 6.99
39 6.99
86.5 6.99
107 6.99
123 9.36
194 9.36
167 9.36
* 9.36
63(27.5) 9- 36
70(20.5) 9.36
Percent Percent
of of
NasCOk. Pyridine.
6.12 23.5
79
96
III
155
196
200+
9.36
9- 36
18. 1
18. 1
18. 1
18. 1
18. 1
18. 1
255
28.4
13.8
15.4
19.5
22.7
25.1
27.6
32.6
8.50
9
II. 4
13.8
16.3
20.1
25
50
2.12
2.25
2.70
4.20
540
6.80
format.
120
132
152
54.2(40.5)
81 (17)
117
142
158
169
180+
64 (26)
78 (18)
106.5
127
148
169
180+
180+
48 (18)
66
79
108
126
155
Precipitate of Na«COa. Results in parentheses show lower temperatures of saturation.
Fusion-point data for NaiCO» + NaCl are given by Le Chatelie (ri894) and
Sackur (1911-12). Results for NajCOs + NaiS04 are given by Le Cfhatelier
(1894), Sackur (1911-12) and by Amadori (1912). Results for NajCOjH- KCl
are given by Sackur (1911-12).
SODroM (Bi) GABBONATE NaHCOt.
SOLUBILm
' IN
Water.
(Dibbits, 1874;
Fedotieff, 1904-)
V
Gms. NaHCO) per 100 Gms.
Water. Solution. '
f.
Gms. NaHCO
per xoo Gms.
w .
Watrr.
Solution.
0
6.9 6.5
30
II. I
10
10
8. IS 75
40
12.7
"•3
20
9.6 8.8
SO
14. 45
12.6
25
IO-3S 9-4
60
16.4
13-8
100 gms. HiO dissolve 9.03 gm. NaHCOi at 15®, dn = 1.061.
(Grecmsh and Smith, 1901.)
100 gms. alcohol of 0.941 Sp. Gr. dissolve 1.2 gms. NaHCOj at 15.5"
100 gms. glycerol dissolve 8 gms. NaHCOs at 15.5**. (Ossendowski, 1907.)
SODIUM (Bi) CABBONATE 638
Solubility op Sodium Bicarbonate in Aqubous Ammonium Bicarbonate
Solutions Saturated with COi.
^
Wt. of I cc.
Solution.
Mols.per looc
NH«HCOk.
» Cms. HflO.
NaHCO»:
Gruns per 1000 Gms. H«(
1^.
NHiHCOk.
NaHCO».
0
1.072
1-39
0.58
109.4
48.2
u
• • •
00
0.82
0.0
69.0
»s
1.056
00
1. 05
00
88.0
«
1. 061
0.29
0-9S
23 0
80.0
If
1.065
056
0.89
44 0
74.6
If
I 073
1.08
0.79
8S-7
66.7
II
1.090
2.16
0.71
170.6
59-2
30
• • •
0.0
I 65
0.0
138-6
II
• • •
2.91
0.83
230
70.0
Solubility of Sodium Bicarbonate in Aqueous Solutions op Sodium
Chloride Saturated with COs.
(Fedotieff; see dao Rekh. 1891.)
t:
Wt. of X oc.
Solution.
MoU.per xooo Gms.HiO.
Unms per xooo Gms. Hfli
NaCl.
NaHCOs. ■
Naa.
NaHCOs.
0
• •
00
082
0.0
69.0
1.208
6.0
009
350 I
7-7
IS
1.056
0.0
I. OS
00
88.0
I 063
0.52
0.82
30. 2
68.6
I 073
1. 03
0.64
60. 1
53-6
1.096
2. 11
0.41
123. 1
34.8
1. 127
3.20
0.28
187.2
23 0
1.158
4 39
0.19
256.9
16. 1
1.203
6.06
0.12
354.6
10. Q
3f
1.066
0.0
I 31
00
II0.2
1.079
1.02
0.87
59 9
72.8
1. 100
2.08
0.56
121. 9
47-3
1. 127
3 18
0.38
186.3
32 0
1.156
438
027
256.0
22.3
1. 199
6.12
O.I7"
358.1
13-9
4S
1.077
00
1.65
00
138.6
l<
1.086
1.04
1. 12
60. 7
94 0
II
1. 115
2.65
062
155-2
52.0
II
1. 127
3 24
0.52
189.4
43-4
II
I 155
4.38
0.37
256.1
30.7
II
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
155^
Solubility of Sodium Bicarbonate in Aqueous Sodium Nitrate
Solutions.
(Fedotieff and Koltunoff, 19x4.)
Gbm. per xoo Gms. H|0.
NaNO,. " NaHCOT
72.74 1.41
29.06 3.40
54-56 2.16
83.20 1.57
95.14 1.80
f.
Sp. Cr. ol
Sat. Sol.
0
I-3S6
IS
1. 183
IS
1-28S
IS
1-377
30
• • •
639 SODIUM GHLORATK
SODIUM CHLORATE NaC10».
Solubility
IN Water.
(Carlson, 19x0; Le Blanc and Schmandt,
1911; <
Osaka, 1903-08.)
f.
dol
Sat. Sol.
Gms. NaaO^ per
zoo Gms. I^.
r.
>
dfA
Sat. Sol.
Gms. NaQ^jper
100 Cms. n/j.
-IS
1.380
72-
40
1.472
126 (xi5LeB.ftS.)
o
1.389
79 (80 LeB.&S.)
50
k . .
140 ("6 «
lO
• • •
89 (87
60
I. 514
15s
IS
1. 419
95 (91
70
■ • •
172
20
1.430
lOI (9S.7 **
80
1.559
189
25
1.44
106 (101 0.)
100
•
1.604
230
30
• • •
113 (xosLeB.ftS.)
122 (
[b.pt.)
1.654
286
The earlier data of Kremers (1856) lie between the values of Carlson and of
Le Blanc and Schmandt.
Solubility op Sodium Chlorate in Aqueous Sodium Chloride Solutions
at 20®.
(Wintelnr, 1900.)
Sp. Gr, of
Gms. per Liter.
s
Sp. Gr. of
Solutions.
Gms.
per.
Uter.
Solutions.
NaCl. NaClOi.
Naa.
NaClOi.
1.426
5 668
w
1.365
175
393
1. 419
25 638
1.345
200
338
1. 412
SO 599
1. 319
225
271
1.405
75 559
1.289
250
197
1.398
100 522
1.256
275
120
1.389
I 25 484
I 235
290
78
1.379
150 442
I. 217
300
ss
100 gms.
HtO dissolve 24.4 gms.
NaCl + 50.75 gms.
NaClOi at 12*
•
100 gms. HtO dissolve I1.5 gms. NaCl + 249
.6 gms. NaClOiat 122'.
(Schk)8ing,i8'
.)
SCH^UBILITY OF SODIUM CHLORATE IN AqUBOUS EtHYL ALCOHOL.
(Carlson, 19x0.)
Gms. NaClOi per liter of Sat. S(d. in Aqueous Alcohol of:
• .
50 Per cent.
75 Per cent
90 Per cent.
20
313-3
II0.8
16. 1
40
321.8
133 -5
22.9
60
326.8
155.8
29
70
...
161. 3
• • •
100 gms. alcohol of 77 Wt. per cent dissolve 2.0 gms. NaClOs at 16^. (Wittstdn.)
100 gms. alcohol dissolve i gm. NaClOs at 25 , and 2.5 gms. at b. pt.
100 gms. glycerol dissolve 20 gms. NaClOs at IS'S**. (Ossendowski, 1907.)
100 cc. annydrous hydrazine dissolve 66 gms. NaClOi at room temperature.
(Welsh and Broderson, 19x5.)
SODIUM PerCHLORATE NaC104.HsO.
Solubility in Water.
(Carlson, 19x0)
ddt
Sat. Solution
Gms. NaQO^
f.
per 100 cc.
Sat. Solution.
Solid Phase.
15
1.666
107.6
NaaO4.Bd0
50
1. 731
123.4
M
143
1.789
141. 4
NaQQi
SODroM CHLOBIDI
SODIUM CHLOBIDS NaCl
640
(Mulder; de Coppet, rSSa^Andne,
1884; Beffcd^
Solubility in Water.
1884; Raupenstnuch, 1S85; above 100*, TSlden
1904; Etard, 1894, gives irregular results.)
and ShenstaoCy
^o G«ns.Naaper GmsJIaa
*L^
Gms.
Naaper
Gms. NaQ
m
xoo Gms. H^.
per
xoo g. 8(4.
0 35-7*
35.63t 26.28t
70
37-8*
37 -Sit
27.27t
10 35-8
35.69 26.29
80
384
38.00
27 54
20 36.0
35.82 26.37
90
39 0
38.52::
27.80
25 36 12
35.92 26.43
100
39-8
39 "t
28.12
30 36 -3
36.03 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
3037
60 37-3
37.06 27.04
180
44.9
30.98
* M.; de C.
t A.
^B.
The original, '
i^ery carefully determined figures
1 of Berkeley, are as foUowsv
*•• a
d of Gms. NaCl per
r.
ddi
Gms. Nad per
St. Sol. 100 Gms. HiO.
Sat. Sol.
xoo Gms. H4O.
0.3s I
•2090 35.75
61.70
I. 1823
37-28
15.20 I
.2020 35.84
75.65
I. 1764
37.82
300s I
. 1956 36 . 20
90.50
I.1701
38.53
45 40 I
.1891 36.60
i07 b
. pt.
I.163I
39-65
100 gms. H^ dissolve 35.99 gins. NaCl at 30"
•
(Cocberet, 1911.)
Solubility of Sodium Chloride in Water, Determined by the Freezing-
POINT
Method.
(Matignon, 19099^)
r.
Gms. NaG
per 100 Gms.
HiO.
Sotid Phase.
f.
Gms. Naa
per 100 Gms. Solid Phase.
H*0.
0.4
0.69
Ice (Raoult)
— 12.7
20
Ice
0.8
1-37
*' (BUU)
~i6.66
25
tt
2.86
4.9
" (Kahleabeig)
— 21.3
30- 7
" +Naa.2Hj0
3 42
5.85
» (Raoult)
-14
32.5
NaCLaHtO (de Coppet)
6.6 .
II
ti
-12.25
32.9
" (BCatignoQ)
9.25
15
it
- 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 subjecti have
been collected by H. Precht and E. Cohn in a volume entitled "Untersuchungen
fiber die Bildungsverhaltnisse die Ozeanischen Salzablagerungen/' Leipzig, 191 2,
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 CHLOBIDS
SOLUBIUTY OF SODIUM ChLORIDB IN AQUEOUS SOLUTIONS SIMULTANEOUSLY
Saturated with Other Salts at 25**.
(vant Hoff, 1905.)
Mob. per xoob Mols. H^.
NatCl,.
KtCW.
MgCli.
MgSO«.
Na«SO«.
I
O.S
105
• • •
• • •
2
5.5
70. 5
• • •
■ • •
44
20
• • •
• • •
4.5
44
10. 5
• • •
• • •
14.5
46
• • •
. • •
16.5
3-0
26
• • •
7
34
4
•
• • •
67.5
12
2.5
• • %
79
9.5
I
• • •
lOI
5
23
14
21. 5
14
19.5
14.5
25.5
14. 5
9.5
9.5
47
14.5
2.5
6
68
5
I
I
85.5
8
42
8
• • •
16
6 '
27.5
10. s
16. s
18. s
22
10.5
23
19
IO-5
7.5
42
19
9
7.5
45
19.5
3.5
4
65.5
13
1.5
2
77
10
I
0.5
100
5
I
0.5
105
• « ■
2
5.5
70. 5
• • •
CaCl^
I
• • •
51.5
90.5
I
II
• • •
140
I
• . •
35.5
121. 5
I
i-S
50- 5
90.5
I
95
5
141. 5
I
2
34.5
121. 5
Solution Saturated with Respect to NaQ and:
MgClt.6HsO + Caroamte
KCl + Camallite
" +Glaserite
NajS04+ "
" + Astrakanite
MgS04.7HiO + Astrakanite
" + MgS04.6HiO
Eieserite + "
" +MgCl,.6H20
KCl + Glaserite + Schanite '
+ Leomte + "
+ " + Kainite
+ Camamte+ "
Eieserite + Camallite + Kainite
NasSOi + Glaserite + Astrakanite
Schonite + Glaserite + Astrakanite
Leonite + Glaserite + Astrakanite
+ MgS04.7H20 + Astrakanite
+ " + Kainite
MgS04.6Hrf) + " +
MgS04.6H20 + Kieserite +
CamaUite + MgCli.6Hrf) +
MgCl2.6HiO + Carnallite
KCl +
it
u
it
it
it
u
ti
tt
MgCl2.6HiO + Tachhydrite
KCl + CaCli.6H,0
Tachhydrite + CaCl2.6HjO
MgClj.6H,0+Tachhydrite+Camallite
CaCl,.6H20 + KCl + CamaUite
CaCl2.6H20 +Tachhydrite + Camallite
Camallite = KMgCI|.6HiO, Glaserite =- K,Na(S04)t, Astrakanite = NasMg-
(S04)i.4HjO, Kieserite « MgS04.H«0, Leonite = MgK,rS04)j.4H,0, SchSnite «
MgKa(S04),.6H,0. Kainite = MgSO4.KCl.3HjO.
Solubility of Sodium Chloride in Aqueous Solutions of Ammonium
Chloride.
(Fedotieff, 1904.)
r.
Wt. of X cc.
Mob. per
xooo Gms. H^.
Cms. per xooo
Gms. HA
Solution.
NH4CI.
NaQ.
NH«C1.
NaCL'
0
• • *
0
6.09
0
356.3
it
1. 185
2.73
4.89
146. 1
286.4
15
1.200
0
6.12
0
357.6
it
1. 191
1.07
558
57.3
326.4
a
1. 183
2.22
5.13
118. 9
300
ti
1. 176
3.48
4.64
186.4
271.6
a
1. 175
3.72
4.55
198.8
266.8
30
• V •
0
6.16
0
360.3
it
1. 166
4.77
4.26
255.4
249
1?
• • •
. 0
6.24
0
365
••
• • •
6.02
4
322.1
233.9
SODIUM CHLOBIDS
642
SOLUBIUTT OF SODIUM CHLORIDE IN AqUEOUS AmMONIA AT $0^.
(Hempel and Tcdesoo, 191 x.)
^of
Gms. per xooocc. Sat. Sol.
Sat. Sol.
Gms. per zooo oc Sat. SoL
SatSoL
NH,.
NaCl. '
' NEU.
NaCL
I. 1735
29. 535
293 38
I. 1406
72.07
283.38
1.1656
40.655
292.5
I . 1395
72.715
283.06
1. 160
47.26
289.7
I.I301
81.855
277.49
I. 1494
60.78
286.5
I. 1205
97-49
270. 57
Data for equilibrium in the system sodium chloride, arsenic trioxide, water, at
30**, are given by Schreinemakers and deBaat (191 5).
Solubility of Sodium Chloride in Aqueous Solutions of Hydro-
chloric Acid.
(Engel, z888; EnUaar, 1901.)
At 0^ (EagelO At I0'*-I0.5^ (Enklaar.)
Mf. Mols. per xo cc
HQ.
NaCl.
0.0
54-7
I.O
1-85
9.28
53-5
52.2
48.5
44-0
IS OS
37-9
30-75
56-35
23-5
6.1
Sp. Or. of
SolttdoQ.
Gms. p
BO.
1.207
0.0
1.204
0.365
1.202
0.674
1. 196
1.859
1.185
3 38
I -173
5-49
1. 141
11.20
1 .119
20.54
Naa.
32-0
31 -3
30-5
28.4
257
22.2
137
3-6
Mob, per liter.
fioT"
0.0
0.27
0.35
0.43
0-57
0.72
2.60
2.80
331
NaQ.
6. II
5-77
5 67
5-59
5-43
5.28
3-42
3.18
2.74
Grams per liter.
Ha. NaQ.
00 35.77
9 84 33 76
12.76 33.19
15.68 32.71
20.78 31.77
26.06 30.89
94.77 20.01
102. I 19.04
120.6 16.03
Results at o^ and at 25''.
(AzmstroDg and Eyre, x9xo-xi.)
Gms. HCl
per Liter
of Solvent.
O
9. II
Gms. NaCl per 100 Gms. Sat. Sol.
Results at 25^. Results at 30**.
(Hers, I9XX-X3.) (Schreinemakers, 1909-10.)
Mols. per Liter. Gms. per xoo GmsJSat. Sol.
18.22
36.45
182.25
4m of
Sat. SoL
I . 2018
I. 1906
I . 1801
1.1633
I. 1512
Ato-.
26.35
25.30
24.15
21.93
At as^.
26.52(^25= 1. 2018)
25.45(<fe6=i.i97o)
25.42(48=1.1915)
22.34(^18=1.1822)
7. 04 (i» =1.1238)
Results at 30*^
Gm. Mob. per Liter.
HCL
0.607
1.032
1.590
2. 117
3.283
NaCL
4.850
4.467
3.782
3.297
2.343
Ha.
o
6.93
12.50
17.35
35.60
NaCl.
26.47
16.16
9-35
4.52
O.II
HCl.
O
0.4575
0.969
1.786
2.412
NaCl.
5-400
4.932
4.386
3.589
2.978
(MasBon, 19x1.)
4m of
Sat. Sol.
I. 1427
I. 1289
I.I188
1.1258
Gms. Mob. per Liter.
HCl.
3.052
4.152
5- 950
7.205
NaCl.
2.463
1.628
0.630
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 Calqum Chloride Solutions
AT 25**.
(MiUs and Welb, X9x8.)
d^of
Sat. So^
1.225
1.233
I. 241
1-257
1.276
d^of
Gms. per xoo Gr
ns. Sat. Sol
Sat. Sol.
CaCl,.
NaCl. '
1.207
1. 103
25.30
I. 210
2.160
24.32
1.209
3.220
23.37
I. 2X6
5.451
20.43
1.220
7.398
19.17
Gms. per xoo Gms. Sat. Sol.
CaClj.
NaCl.
9.50
17. 55
11.48
15.91
17.77
10.54
21
8.05
24.58
563
643
SODIUM GHLOBmS
SoLUBiuTY OP Sodium Chloride in Aqueous Potassium Nitrate at 25/
(RitaeU 19x1)
Cms. per xoo cc. Sat. Sol. Gms. per xoo oc. Sat. SoL
KNOi.
NaCl.
KNO,.
NaCl.
0
31-80
12
30.86
4
32.26
16
30.4s
8
. 3i.8s_:
20
30.10
Data for the solubility of NaCl in aqueous MgCU solutions are given by Feit
and Przibyila (1909.)
Solubility of Mixtures op Sodium Chloride and Other
Salts in Water, etc.
Authority.
(Kantea.)
Solvent.
17
Gnu
■ per 100 Gnu. Solvent.
Water
36.4
NaCl+3a.iNH«Cl*
i(
17
34-5
" + 4iBaCl,
fi
?
383
" +39.5 KNO,
it
25
385
" +41 14 "
it
80
39.81
« +168.8 "
Alcohol (40%)
25
15 78
" +13-74 "
Water
30
30 54
" +13.95 KCl
" +16.12 "
((
25
38.90
•t
(Soch — J. Phyaic. Ch. 3, 46, '98.)
<t
(Quoted by Euler — Z. phyaik. Ch.
40, 31S, '04.)
* Sp. Gr. of solution at 17" ■- 1.179.
SOLUBIUTY OF MIXTURES OF SODIUM CHLORIDE AND POTASSIUM SULFATE
IN Water at Various Temperatures.
(Precht and Wittgen, 1883.)
Ao Gmms per 100 Grams HjO. ^o Grams per xoo Grams HsO.
10
20
30
40
SO
NaQ
33-4
34 o
34-6
35-2
3S-8
K1SO4
8.1
8.9
9.6
10.4
II. I
Kci
3-2
31
2.9
2.8
2.8
60
70
80
90
100
NaQ
36 -4
36.6
36.0
3S-9
3S-6
K9SO4
II .9
12.8
12.3
12.4
12.6
KCl
2.7
3-2
S-i
7.0
8.8
Solubility of Sodium Chloride in Aqueous Solutions of Sodium
Bicarbonate Saturated with COi. (Fedotieff 1904.)
r.
o
((
IS
30
45
Wt. of X cc.
Solution.
1.208
1.203
1.203
1. 196
1. 199
1. 189
1. 198
Mols. per xooo Gms. H^.
NaHCOk.
O
0.09
O
0.12
O
0.17
O
0.23
NaQ.
6.09
6
6.12
6.06
6.16
6.12
6.24
6.18
Gms. per xooo Gms. H|0*
NaHCO,.
O
O
10
o
13 -9
o
19s
NaQ.
356.3
3SO.I
357.6
354.6
360.3
3S8.I
36s
361. S
Solubility of Sodium Chloride in Aqueous Sodium Hydroxide at 3o^
^(SchreinemakerB, X909-X0, xqxo.)
Solid Gms. per xoo Gms. Sat. SoL
Phase. Na,0. ' NaCl.
NaQ 29.31 2.40
Gms. per xoo Gms. Sat. Sol.
Na«0.
NaCl.
0
26.47
4.47
21.49
12.22
13.62
24.48
4.36
Solid Phase.
NaQ
i<
(I
37 -85
41.42
zk42
1. 12
0.97
O
*i
" +NaOH.H/)
NaOH.HsO
SODIUM CHLOBIDS
644
SCX.UBILITY OF Sodium Chloride in Aqueous Sodiuu Hydroxide
Solutions.
(Engd; WtDtder, 1900.)
At 0' (Engei;
1.
At 20
• (Winteler).
Mg. Mols.
per 10 cc.
NaCl.
Sp. Gr. of
Sdutiona.
Cms. per Liter.
Gibs, pei
r liter.
Sp. Gr. of
N.,0.
NaOH.
NaCL
NaOH.
NaCl.
' SolutkKB.
0
54. 7
1.207
0
320
10
^08
1.200
4-8
4938
1. 221
38.4
288.9
SO
297
1.230
6-73
47.21
1.225
53-8
276.2
100
253
1.250
10.41
42.38
1.236
183.2
247.9
150
213
1.270
14.78
39 55
1.249
118. 2
231.4
200
173
1.290
30-50
24.9s
1.295
244
146
300
112
1.330
37.88
19.30
1. 314
303
IT2.9
400
61
1-375
53-25
9.4J
1.362
426
55
SOO
640
30
18
1.425
1.490
Solubility of Sodium Chloride in Aqueous Solutions of Sodium
Nitrate and Vice Versa.
NaCi in Aqueous NaNOi.
NaNOi in Aqueous NaCl.
Results at i
^5.5' (B.)
.
Results at
15' (B.).
Sp. Gr. of
Gins, per
zoo cc*. Sat.
Solution.
Sp. Gr. of
Gms. per
100 cc. Sat. Solution.
SdutioQS.
NaNO,.
H2O.
NaCl.
Soludon*.
NaCl.
HsO. NaNOs.
1.2025
0
88.47
31-78
1.37*0
0
74.82 62.38
1-2305
7-53
87.63
27-89
I .3645
4.0
75 69 56.76
1.2580
13-24
86.25
26.31
1-3585
7.24
75-71 5209
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
1-3345
33-80
79-25
20.40
I -3485
17.81
77.14 3990
1 .3465
37-88*
77-37
19.40*
I -3485
18.97*
77-15 38 -73*
1-3465
37-64*
77-34
19.67*
I 3485
19-34*
77.49 38.02*
Results at 20° (N.).
Grams per 100 Grams HaO.
Grams per xoo Grams H2O.
0 NaNO,
35.91 NaCl
0 NaCl
87.65 NaNO,
14-17 "
32-82 "
6-5 "
77-34 "
28-33 "
29-78 "
13-0 "
68.50 *'
42-50 "
86.91 "
19-5 "
60.49 "
54-63* "
24.92* "
100 gms. H2O dissolve 43.66* gms. NaNOi + 26.58* gms. NaCl at 25®.
100 gms. HjO dissolve 121.6* gms. NaNOi -f 17.62* gms. NaCl at 80®.
100 gms. aq. alcohol of 40 wt. per cent dissolve 22.78 gms. NaNOi + 10.17 gms.
NaCl at 25^
* Indicates solutions saturated with both salts.
645
SODIUM CHLOBIDS
SoLUBiLmr OF Sodium Chloride in Aqueous Solutions of Sodium Nitrate
AND Vice Versa.
(Leather and Mukerji, 19x3.)
Results at 30**.
4m of
Sat. Sol.
Cms. per 100 Cms.
NaNOk. NaQ.
o 36.3
24.21 31.16
48.15 26.35
63.08 23.50
63.40 23.40
67.91 19.69
81.46 9.76
Sat. Sol.
Results at 40°.
Cms. per xoo Gms.
2(2:
202
276
343
379
388
381
394
406 95.90 o
1. 197
1.284
1.323
1.409
1.397
1.396
1. 410
1. 421
NaNO,.
o
27.31
54.82
73.96
74.01
75.29
NaCl.
36.53
30- 53
26.50
21.87
21.71
2L.6l
89.90 10.80
105 . 2 o
(in of
Sat. Sol.
.189
.296
•381
.487
.519
.518
Results at 91"^.
Gms. per xoo Gms.
H/).
NaNOk.
O
37.43
79-65
127. 2
141. 4
141.3
.504 149.5
.521 160.8
NaCl.
38.72
30.21
23.17
17.05
15-93
15-83
903
o
Solid Phase
in Each Case.
NaQ
(I
M
41
" fNaNO,
" NaNOi
u
i<
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 0° and at 25° are given by Armstrong and Eyre (1910-11).
Solubility op Sodium Chloride in Aqueous 7.45 Per cent Sodium
Sulfate Solutions.
(Marie and Marquis, 1903.)
r.
Gms. NaCl per
M Qma. ^
* • xoo Gm
faGper
xoo Gms. Sat. Sol.
s.Sat. SoL
14.8
23 30
27 -75 23
.525
17.9
23 -33
32.18 23.55
25.6
23.485
34 . 28 23
.68
For additional data on this system
see sodium sulfate, pp. 669 and 670.
Solubility
OF Sodium Chi.oride in Aqueous Solutions
Alcohol.
(Armstrong and Eyre, 19x0-1 x.)
OF Ethyl
Results at 0**.
Results at 25*.
Solvent Gms.
Gms. NaQ
^ ^, Solvent Gms.
Gms. NaCl
CH.OHper
1000 Gms. afi.
per zoo Gms.
Sat. Sol.
per xoo Gms.
Sat. Sol.
0
26.46
I . 202 0
26.55
II. 51
25-97
I. 196 II. 51
26.06
23-03
25-48
1. 190 23.03
25 63
46.06
24.41
1. 179 46.06
24.75
138.18
20.95
I. 159 92.12
23.29
I.III5 230.3
19.35
Solubility of Sodium Chloride in Aqueous Alcohol at 28^.
(Fontein, xgxo.)
Gms. per xoo Gms. Sat. Sol.
Gms. per xoo Gms. Sat. Sol.
(^HgOH.
B|0.
NaCL
0
73 53
26.47
3-8
71.6
24.6
7-7
69:7
32.6
16. 1
64 .6
193
2S-3
58.9
iS-8
35
525
"•5
CiHiOH.
H,0.
Naa.
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 CHLOBIDl
646
Solubility op Sodium Chloride in Alcohols.
(At 18.^, de Brayn — Z. physk. Ch. lo^ 78a, '9a; Rnhland — Z. anorg. Ch. i8t srj, V8-)
u
Alcohol.
18.5 Abs. Methyl
" Ethyl
Cms. N&Cl
per 100
Cms. Alcohol.
1. 41
0.065
room temp.
((
it
Gins.Nfta
Alcohol per xoo
Gms.AlcohoL
Methyl i^-o .799 i .33
EthylJ,5 =0.81 0.176
Propyl di^ — o .816 o .033
Solubility op Sodium Chloride in Aqueous Ethyl Alcohol
Solutions.
(Bodlinder — Z. physik. Ch. 7, 3x7, '91 ; Taylor — J . Phys. Ch. i, 723, '97; alao Bathridc — Ibid. i.
Restiltsat 11.5° (B.).
Results at 13® (B.).
Sp. Gr. of
Soltttiopa.
2035
1865
1710
1548
1350
1390
1088
Gms. per xoo cc. Soludon.
CsH^U.
O
2.86
S-4I
7-93
10.84
11.22
16.85
HsO.
86.62
86.14
^3-93
81.50
78.78
78.62
73 40
NaQ.
31 -73
29.66
27.77
26.05
24.28
23 65
20.63
Sp. Gr. of
SoludoDs.
I . 2030
I . 1348
I.II44
1.0970
1.0698
I .0295
0.9880
09445
0.9075
0.8700
0.8400
Gms. per xoo cc. Solution.
CaHsOH.
O
II
IS
19
24
32
40
49
57
63
72
Results at 30** and at 40° (T.)
Wt. per cent
Alcohoiin Solvent.
O
5
10
20
30
40
SO
60
70
80
90
At 30*, Gms. NaCl per loo Gms.
At 40**, Gms
81
99
39
95
33
33
28
91
86
26
HaO.
88.70
78
74
71
65
57
49
38
29
21
II
41
64
45
80
96
34
54
37
62
24
KaQ.
31 60
23.26
20.81
18.86
16.23
12.66
913
5
3
I
93
47
52
0.50
NaClper xooGma.
Solutiooi.
26.50
24 -59
22-66
19.05
15-67
12.45
9 34
6.36
3 36
1.56
043
Water.
36 05
34
32
29
26
23
20
16
12
7
4
29
57
40
53
70
60
96
75
95
30
Soluticm.
26.68
24.79
22.90
19.46
16.02
12.75
9.67
6.65
3 87
1.69
0.50
Water.
36.38
34 69
33'^
30.20
27.25
24-37
21.42
17.82
13.10
8.68
5.10
100 gms. alcohol of 0.9282 Sp. Gr. = 45.0% by wt. dissolve at;
4^ 10^ 13'' 23^ 32^* 33^ 44^ 51^ *6o«
10.9 II. I 11-43 11-9 12.3 12.5 13. 1 13.8 14. 1 gms. NaCl
(Gerardm — Ann. chim. phys. [4] S 1461 '56O
100 gms. of a mixture of equal parts of 96% alcohol and 98% ether
dissolve o.ii gm. NaCl.
(Mayer — Liebig'a Ann. 98» 905. 'j60
647 SODIUM CHLOBIDl
SOLUBILXTT OF SODIUM CHLORIDE IN AqUBOUS MbTHYL AlCOHOL.
(Annstrong and Eyre, igzo-xi.)
Results at o^. Results at 25^.
Solvent, Cms. Cms. NaCl Solvent, Cms. Gms. NaQ
CHjpa per per 100 Gms. C^OH per per 100 Cms.
zooo Gms. 11^. Sat. SoL 1000 Cms. H^. Sat. SoL
o 26.35 S-oi 26.29
8.0Z 36.05 16.02 26.02
i6.oa 25.79 32.04 25.50
32.04 29.19 96.12 23.50
A sat. solution of NaCl in CHaOH contains o.i gm. NaCl per 100 gms. solution
at the critical temperature. (Centnexszwer, 191a)
SOLUBILITT OF SODIUM ChLORIDB IN AqUEOUS PrOPYL AlCOHOL.
(Armstrong and E3rxe, 19x0-11.)
Aqueous propyl alcohol containing 15.01 gms. C1H7OH per 1000 cc. H^ dis-
solves 25.71 gms. NaCl per 100 ^s. sat. solution at o^ and 25.95 gms. at 25**.
Aqueous propyl alcohol containing 30.02 gms. CsHtOH per 1000 cc. H2O dis-
solves 25.12 gms. NaCl per 100 gms. sat. solution at o® and 25.37 S^^s. at 25°.
Equilibrium in the System Sodium Chloride, Normal Propyl Alcohol
AND Water at 23-25**.
(Frankforter and Frary, 19 13.)
The authors detennined the binodal curve and quadruple points of the system
but did not locate tie lines.
»
Cms. per 100 Gms. Homogeneous Liquid. Gms. per xoo Gms.|Homogeneous liquid.
/ * N
HtO.
"75*
46.20
77.46
81.32
81.96
82.47
81.72
81.23
* 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 CsHtOH contain 0.04 gm. NaCl
at 25°. (Frankforter and Frary, 1913.)
EQUmiBRIUM IN THE SYSTEMS SODIUM CHLORIDE, AlLYL AlCOHOL, WaTER, AT
20° AND Sodium Carbonate, Allyl Alcohol, Water, at 20°.
(Frankforter aiui Temple, 19x5.)
Results for Results for
NaCl + CH, : CHCHjOH + HjO. NaiCOi + CH, : CH.CH,OH + H,0.
Naa.
CtHTOH.
o.SS
87.7
2.23
51.57
3-55
18.99
3.90
14.78
5- 27
12.77
8.04
9.49
10.49
7.79
12.20
6.57
kaa.
CHtOH.
h^.'
14.38
5.39
80.23
15.42
5."
79.47
16.38
4.47
79-14
18.08
3.83
78.09
20.12
3.27
76.61
22.35
2.64
75.01
24.50
2.13
73.37
24.9
2.3
72.8*
Gms. per
xoo Gms. Alcohol + Water.
A
Gms. per
xoo Gms. Alcohol + Water.
A
NaCl.
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. Oil
51.930
48.070
6.712
54.683
45.317
1.468
48.109
51.891
8.776
47.132
52.868
2.580
41.052
58.948
10.650
40.392
59.608
3.414
37.126
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
i«.557
19.705
80.295
10.079
18.407
81.593
SODIUM GHLOBIDl
648
Solubility of Sodium Chloride in Several Alcohols at 25^
Cluiner and Biaaett» 1913.)
Alcohol.
Methyl Alcohol, CH,OH
Ethyl Alcohol, CiH»OH
Propyl Alcohol, CsHyOH
Amyl Alcohol, CsHnOH
Gms^ NaG per
zoo Gms. Aloobol.
1. 31
0.065
0.012
0.002
SoLUBiLmr OF Sodium Chloride in Aqueous Acetone Solutions at 20^.
(Frankforter and Cohen» 1914.)
Gms.
per 100 Gms. Sat.
SoL
GnM.
per xoo Gms. Sat. Sol.
NaCl.
H,0.
(CH,),CO.
. NaCl.
H,0.
(CH,),CO.
25-9
73.06
1.04
16.55
61.59
21.86*
24.19
71.18
4.03
0.4s
13.75
85.8*
20.85
66.78
12.37
0.32
13-92
85-76
18.32
63.16
18.52
0.19
10.82
88.99
17.89
62.21
19.90
0.12
8.94
90.94
* Quadpt
Between the concentration 21.86 and 85.8 per cent acetone, two layers are
formed. The bincxial 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:
Gms. per zoo
Gms. Homogeneoius liquid.
Gms. per
100 Gms. Homogeneous Liquid.
NaCl.
HA
(CH|),CQ
NaCl.
H,0.
(CH,),C0.
0.59
15.46
83.95
5.87
40.19
53.94
0.79
17.58
81.63
6.45
42.12
51.43
0.93
18.83
80.24
7-53
46.12
46.3s
1.27
22.19
76.54
8.87
49.39
41.74
1.57
23.89
74.54
9-47
50.92
39-61
2.31
27.27
70.42
to. 35
53.06
36.59
4.87
36.79
58.34
15.87
59.71
24.42
Additional data, showinsr the effect of temperature on the above system, are
also given
Solubility of Sodium Chloride in Aqueous Solutions of:
Acetone at 20®.
(Hers and Knoch, 1904.)
cc. Acetone NaCI oerzoo cc.
oerxoocc. Solution.
Glycerol at 25**.
(Herz and Kaooli, 1905.)
Wt. Per cent NaCl per 100 cc
Glycerol in SoluUon.
Solvent. Slillimob. Gms.
0 545.6 31.93
13.28 501. I 29.31
25.98 448.4 26.23
45.36 370.2 21.66
54.23 333-9 19-54
83.84 220.8 12.91
100 * 167. I 9.78
Sp. Gr. of
Solution.
I. i960
1 . 2048
I. 2133
I . 2283
I. 2381
1.2666
I . 2964
Solvent.
0
10
20
30
32 Lower layer
87 Upper layer
90
MiUimols.
537-9
464.6
394.8
330.1
308.5
7.7
7.3
4.3
Gms.
31.47
27.18
23.10
19.32
18.05
0.45
0.43
0.25
* Sp. Gr. of Glycerol, 1.3593. Impurities about 1.5%.
100 gms. sat. solution in glycol contain 31.7 gms. NaCl at 14.8''.
(de Coninck, 1905.)
100 gms. HsO dissolve 236.3 gms. sugar + 42.3 gms. NaCl at 31.25**, or 100
gms. sat. aq. solution contain 62.17 gms. sugar + 11. 13 gms. NaCl. (KOhler» 1897.)
649
SODIUM CHLOBmS
Equilibrium in the System Sodium Chloride, Methyl Ethyl Ketone
AND Water at 25** (Binodal Curve).
(Frankforter and Cohen, 1916.)
Gms. per 100 Cms. Homogeneous Liquid.
NaQ.
0-3S
o-SS
1.42
1.80
2.47
4. II
CH,.C0.CH,.
20.13
19 -75
16.52
17.70
16.24
13-34
HaO.
79 52
79.70
82.06
80.50
81.29
82.5s
Gms. per xco Gms. Homogeneous Liquid.
NaCI.
6.7s
10.07
14.32
14 65
23. IS
24.14
CH,.C0.C»H».
10.80
7-65
536
3.83
2.08
0.94
H,0.
82.45
82.28
80.32
81.52
74.77
74.92
Solubility of Sodium Chloride in Aqueous Solutions of Carbamide
(Urea) and of Formamide at 25**.
(Ritzd, 191 1.)
In Aqueous Carbamide.
In Aqueous Formamide.
Gms. C0(NHt)j
GmK. NaCl
Gms. HCO.NHt
Gms. NaO
per 100 cc.
per 100 cc
per 100 cc.
per xoocc.
Solution.
Solution.
S<^ution.
Solution.
0
3180
0
31.80
S
30-63 .
2.3
30.98
9.6
29.05
S-3
30.86
13
28.46
8
30.40
18
27.65
II
29.11
23
27.24
IS
28.52
28
26.56
18.8
27.76
According to results by Fastert (1012), the solubility of sodium chloride in
aqueous solutions of urea mcreases slightly with increase of urea in solution, thus:
Gms. CO(NH2)2 per 100 cc. Sol. 10 20 30 40 50
Gms. NaCl per 100 cc. Sol. 31-92 32.17 32.51 32.93 33.40
Data for eouilibrium in the system sodium chloride, succinic acid nitrile, water
are given by Timmermans (1907).
100 gms. 05% formic acid dissolve 5.8 gms. NaCl at 19.7°. (Aachan, 1913.)
100 gms. hydroxylamine dissolve 14.7 gms. NaCl at 17.5^. (de Bruyn, 1892.)
100 cc. anhydrous hydrazine dissolve 8 gms. NaCl at room temp.
(Welsh and Brodenon, 1915.)
Fusion-Point Data (Solubilities, see footnote, p. i) Are Given for the
Following Mixtures.
NaCl + HC!.
" + NajCr04.
" + NaCN.
" + NaF.
" + NaOH.
" + Nal.
" + NaNO,.
" + Na4Pt07.
" + NajS04.
" + SrCl,.
" + SrCOi.
" + TlCl.
(Demby, 1918.)
(Sackur, 19x1-13.)
(Truthe, 1912.)
(Ruff and Plato, 1903; Wolters, 19x0; Plato, X907.)
(Scarpa, 19x5.)
(Ruff and Plato, X903; Amadori, 19x20.)
(Meneghini, X9X2.)
(LeChatelieT, 1894.)
(Ruff and Plato, X903; J&necke, X908; Wolters, x9xo; Sackur, X9xx-i9.)
(Vortisch, 19x4; Sackur, X9xi-X2.)
(Sackur, X91X-X2.)
(Sandonnini, x9xi, 19x4.)
SODIUM CHROMATIS 650
SODIUM CHROMATIS (Mono, Di, etc.)
Solubility in Water.
(Mylius and Funk, 1900; lee aho Salkowski, 1901.)
Sodium Monochromate. Sodium Dichromate.
Gms. Naa Mob. Na*
Cr04 per CrO.
100 Gms.
Solutkn.
U per
zoo Mols
HsO.
Solid
Phaie.
Gms. Naa
CrsOfper
xoo Gms.
Solutioa.
Mols. Nas
[<Ss
CrsOr per
:oo Mc'
O
10
18*
18.5
21
25.6
31-5
36
40
45
49-5
54-5
59-5
65
70
80
100
24.07
33-41
40.10
41.65
44.78
47 -40
46.08
47-05
47.98
48.97
50.20
50 -93
52.28
53-39
55-23
55-15
55-53
55-74
3.52Na4CrQc.xoH^ O
5-55
7-43
7-94
9.01
10.00
M
17
i8t
34-5
52
7i
9.52NaaCrO«.4HaO 8l
9.90 " 93
10. :« '• 98
10.6 ••
II. 6 "
"•5 - t«
Ii.2 ••
12.7 -
13-7 NaaCrOi
13.6
13-8
14.0 "
61
63
63
67
71
76
79
81
81
98
82
92
36
76
9
8
19
25
100
HaO.
II. 2
12. 1
12.16
14.2
17-4
22.8
27.1
29.6
29.8
Solid
Phase.
Na«CnOr.aB^
NasCisOr
O
i5t
18
55
99
Sodium Tri Chromate.
Gms. Nas Mols. Nas
CriC^ per CriOio per
xoo Gms. xoo Mols.
Soludoo. HsO
.80.03 19-9
80.44 20.4
80.60 20.56
82.68 23.7
85.78 29.9
Solid
Phase.
NasCi«0||.HgO.
* Sp. Gr. of sat. sol. at x8* - x.439. t Sp. Gr. of sat. soL at xS** 3.059
X Sp. Gr. of sat. solutioo at x8* ■■ 1.745.
Sodium Tetrachromate.
Tetraaodium. Chromate.
Gms.
.• ' Na^40is
* '- per xoo Gms.
Solutioo.
Mols.
NasCr40is
per 100
Mrils.HaO.
Solid
Phase.
Gms.
*. Na^CrOs
' per xooGms.
Solution.
Mols.
Na^CrOs
per xoo
M^.HflO.
Solid
Phase.
0 72.96
10.5
NasCr^Oxs^HsO
0 33-87
4. II 1
7adCrCVx
16 74-19
i8* 74.60
II. 2
11.27
M
M
10 35.58
i8t 37 50
4.42
4.81
M
M
32 76.01
12.3
M
27.7 40.09
37 45-13
5-38
6.62
H
• •
* Sp. Gr. of sat. solutioo at x8*«i 1.936.
t Sp. Gr. of sat. solution at xS*"* x.446.
A new hvdrate of sodium chromate, NasCr04.6HiO, was found by Salkowskiy
(1901) and the following data for its range of existence were determined.
Gms.
Mols.
Gms.
Mols.
Na«CiO«
Na«Ci04
Na,CiO«
Na.Ci04
f.
per xoo
per xoo SoUd Phase.
f.
per
per Solid Phase.
Gms.
Mols.
zoo Gms.
xoo Mols.
Solution.
H,0.
Sol.
H,0.
17.7
43.65
8.62Na,CiO«.xoH/)
25. 9
46.3*
9.57Na*Ci04.6HdO
19.2
44.12
8.77 "
+NaaCiO«4H^
19.525
44.2*
... " +Na,Ci04.6H,0
28.9
46.47
9.64Na/:i04^BV)
21.2
44.64
8.96 Na,Ci04.6H^
29.7
46.54
^'H I
24.7
4575
9.37
31.2
47.08
9.88
• This determination by Richards and Kell^ (i9")'
651
SODIUM GHB0MATE8
Solubility of Sodium Chromates in Water at 30^
(SchrrincmakerB, 2906.)
Composition in weight per cent:
Of Solution. Of Residue.
%CrO».
%Na«0.
%CKh.
%NaiO.
Solid Phase.
0
±42
...
• • •
NaOH.HsiO
2.00
41.44
5-83
42.64
NaOH^sO + NaiOQi
2.04
40.89
...
...
NaflCrO«
423
35 51
27.52
3^-57
M
6.64
32-34
27.72
34.60
M
15 19
27.06
37-07
32.20
tt
10.22
29 -39
15-48
28.41
NasCrO« + Na4Cr05.X3H«0
«-93
28.49
18.09
26.89
NaiCrOA.z3HaO
8.62
26.91
« • •
• • •
M
13 12
23.91
x8S7
25.92
M
18.44
22.86
■ • •
• • •
M
19.26
2^.98
21.54
25-31
Na«CrOs.x3HsO + NajCiO«^H«0
17.84
24.21
26.24
24.98
Na4CrO«4HaO
28.82
17.88
31-97
23-47
M
38-93
16.30
40.70
20.83
M
48.70
16.49
47-49
19-75
NasCr044HiO + NasCr«Or.aH«0
50.68
15-72
• • •
• • •
NasCrsOr.aHaO
58.08
13.89
6s. 76
17-38
u
66.13
13-70
69.48
16.06
Na«Qri07.9HsO + NaaCc«Oxo.HaO
65.98
14-15
69.46
15-15
NaaOiO]O.HiO
68.46
10.95
73-88
^3-3^
NaflCraOicHaO + NasCr«Qii4HiO
66.88
9-85
71.27
10.67
Na«Cr«Qtf4H^
70.06
11.85
83-95
9-57
"(?)
69.04
11.04
81.80
6.43
CrOa
67.84
9.81
82.85
5-42
M
64.48
4.51
79-49
2.71
M
62.28
0.0
• • •
U
100 gms. of a saturated aqueous solution contain at 30^:
46.627 gms. Na2Cr04, or 100 gms. HsO dissolve 87.36 gms. NasCr04.
66.4 gms. NasCrsOr, or 100 gms. HsO dissolve 197.6 gms. NasCriOr.
100 gms. absolute methyl alcohol dissolve 0.345 gms. NasCr04 at 25**.
(de Brayn, 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 CHB0MATE8 652
Solubility of Sodium Dichromatb in Alcohol at 194^
(Rdnitzer, 1913.)
r
* An excess of NasCrf07.3HfO was shaken with absolute alcohol for 10 minutes
and the mixture filtered. The filtrate contained 5.132 gms. NaiCrs07.2HiO per
100 cc. and its duA was 0.8374. '^^^ solution decompoKd 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 CeH»CH:CHCOONa.
100 gms. HsO dissolve 9.1 gms. sodium cinnamate at 15.20®.
100 cc. 90% alcohol dissolve 0.625 gm. at 15-20**. (Squize ud Cuan, 1905^
SODIUM CITBATE (CHs)sCOH(COONa)t.5}HsO.
Solubility in Aqueous Ethyl Alcohol at 25®.
(SeideU. 19x0.)
Wt. Percent ^ ^m Gms. CAOrNa*.- Wt. Percent 3 ^« Gms. CAOrNa«^
qiLOHm cfTcLi siHdOperxooGms. QHtOHin c^cli SiHsOperiooGms.
Sofvent. Sat. Sol. ^'"^sktSoL Solvent Sat.SoL *' « sit SoL
o 1.276 48.1 40 0.953 45
10 1. 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 o
Data for equilibrium in the system sodium hydroxide, citric acid, phosphoric
acid and water at 20^ are ^ven by Pratolongo (1913).
The author fails to describe clearly the terms in which the results are ezpresaedp
consequently their exact meaning is not clear.
SODIUM (Ferro) CYANIDE Na^FeCCN)..
Solubility in Water.
(Conroy, 1898.)
f. 2o*. 4a*. 8o». 98.S*.
Gms. Na4Fe(CN)6 per loo gms. HjO 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 zooo Gms. H|0. Gms. per zooo Gms. HaO*
o HF 41.7 NaF 83.8 HF 22.9 NaF
10 " 41-4 " 129-7 " 23 -8 "
45. 8 " 22. s " 596.4 " 48.8 "
56.S " 22.7 « 777-4 " 81-7 "
Fusion-Point Data (Solubility, see footnote, p. i) Are Givbn for the
Following Mixtures.
NaF + FeFt. (Puschin and Baskov, 19x3.)
" +ZnFi.
II
<i
+ Nal. (Ruff and Plato, x903*)
4- NaOH. (Scarpa, 1915.)
" + NajS04. (Wolters, X9XO.)
SODIUM nUOSILICATE Na^SiFe.
100 gms. HiO dissolve 0.65 gm. at 17.5*. and 2.45 gms. at loo^ (Stdbm iSrad
653
SODIUM FORMATE
SODIUM FORMATE HCOONa.
Solubility
IN Water.
(GxoKhuff. 1903.)
Gms.
♦• HCOONa
* periooGma
Soludoa.
Mob.
HCOONa
perxooMolfl
HaO.
SoHd
Phase.
Gms.
^» HCOONa
' perxooGma.
Solutioa.
Mob.
HCOONa
perxooMob
HjO.
Solid
Phase.
— 20 22.80
7.82
HCOONa.3HsO
^SS SOS3
27.0
HCOONa.aH|0
0 30. 47
II. 6
M
18 49-22
25-65
HCOONa
+ 15 41 -88
19. 1
M
29 50.44
26.9
M
18 44*92
21.6
M
54 S3 80
30. 8
«
18 44.73
21.4
HCOONa.aHaO
74.5 S6-82
34.8
M
21 46.86
23 -3
M
1005 61.54
42-35
M
23 48.22
24.65
M
123 66.20
51 -8
M
Sp. Gr. of the sattirated solution of the dihydrate at 18** « 1.317.
Solubility op Sodium Acid Formate (Expressed as Neutral
Salt) in Aqueous Solutions op Formic Acid.
(Groflchuff.)
Gms. Mob.
Solid ^c
Phase. *
Gms. Mols.
HCOONa HCOONa
perxooGms. periooMob-
66.5
Solatioo.
22.35
29.62
41.08
HaO.
19-5
28.45
47.1
HCOONa HCOONa Solid
perxooGmt. perxooMob. Phase.
SoludoD. HsO.
HCOONa.HCOOH
45 S
38-85
43 I
HCX>ONa
70
41.27
47 5
M
85
43 09
SI .2
SODIUM QLTCEBOPHOSPHATE (Disodium) OP(OC«H70s)(ONa)s.5H,0.
100 gms. sat. solution in HiO contain 27.38 gms. of the anhydrous salt at 18®.
(Rogier and Fiore, 19x3.)
SODIUM HTDBOZZDE NaOH.
Solubility in Water.
Gms. NaOH
*•.
per xoc
> Gms.
Sdutian.
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
43.0
+ 5
32.2
47 5
10
34.0
51 5
155
38.9
63 -53
5
45-5
835
12
50.7 103.0
(Pickering, 1893; Mylius and Funk (Diets), 1900.)
Cms. NaOH
%•, per xoo Gms.
Siolution. Water.
SoBd
Phase.
Ice
20
30
40
SO
60
64
loe+NaOH.rHsO
NaOH.rHsO +NaOH.5H|0
NaOH.sHsO + NaOH^H^ a
NaOH^HsO «
NaOH^HaO a+ NaOH3iHsO 61
NaOH.3iH30 80
f. pt. no
NaOH.3iH^+NaOH.aH|0 jqq
NaOH.aH30+ NaOH.H|0
52
54
56
59
63
369
874
75
78
83
2
3
3
2
5
o
2
8
5
9
109
119
129
145
174
222
288
313
365
521
Solid
Phase.
NaOH.H|0
-f.pt.
NaOH^HsO
+ NaOH
NaOH (?)
Sp. Gr. of sat. solution at 18^ » i*539-
For determinations of the Sp. Gr. of sodium hydroxide solution, see Kohlrausch^
1879; W^;scheider and Walter, 1905.
100 gms. of the sat. solution in water contain 46.36 gms. NaOH at 15^.
(de Forccand, 1909^*)
SODIUM RTDBOZZDB
654
1000 gms. liquid ammonia dissolve 0.0025 P^* NaOH at —40^
(SkoMamwky and Trliifriiinadir, <9i6.)
Data for equilibrium in the system sodium hydroxide, resorcinol and water at
30° are given by van Meurs (19 16).
Fusion-point data for NaOH + Nal are given by Scarpa (1915).
SODIUM lODATE NalO..
SqLUBILITT in WaTBK. (Gfty-LoMc:
2-5
.iSsfia.)
9 IS 21
80*. 100*.
27 34
Gms. NalQt per 100 gms. H^
Equilibkium in thb System Sodium Iodatb, Iodic Acid and Water at 30^
(Meerbuig, 1905.)
Gms. per 100 Gms. Sat. Sol.
HlOb.
O
1.98
4.86
S.86
7.40
9-73
6.70
7.80
9.15
9.93
NalOi.
9 36
9S2
10.22
11.04
11.60
14.73
II. 21
10.30
9
8.71
Solid Phase.
NalCViiH/)
Gms. per 100 Gms. Sat. ScA,
u
«
«i
If
M
tuHtable
11
" +N%0.aIA
Na^.aIA
(4
M
HlOb.
11.20
11.82
11.62
23.23
32.68
46.62
ss. 48
65.47
76.19
76.70
NalOi.
7. 54
7.20
5.65
369
2.91
2.67
2.12
1.83
1.42
o
Solid Phase.
Na^.3lA
" +NaIOb.aHIO^
NaIOb.aHIOb
M
+HIOb
m(\
SODIUM IODIDE NaI.2HiO.
SoLUBiLmr IN Water.
(de Coppet, 2883; see also Etaid, 1884; and Kremers, x8<(6a.)
f J
jrams NaT
per 100 Gms
Solid
Phase.
t».
Grams NaJ
[ per 100 Gms
• . ^"
Water.
Solution.
Water.
Solution.
—20
148.0
59-7
NaI.aH30
60
256.8
72.0
0.
158-7
61.4
u
65
278.4
73-6
10
168.6
62.8
M
67
293
74.6
20
178.7
64.1
M
70
294
74.6
25
184.2
64.8
«
80
296
74.7
30
190-3
65.6
W
100
302
75 1
40
205.0
67.2
M
120
310
75-6
so
227.8
69 -5
W
140
321
76.3
Solid
NaI.aHaO
Nal
The eutectic mixture of Ice + NaI.5HiO is at —31.5^ and contains about 39
per cent Nal. (Meyerhoffcr, 1904.)
The tr. pt. for Nal.sHiO + NaI.2HsO is at —13.5 and the saturated solution
contains 60.2 gms. Nal per 100 gms. (Paafiloff, 1893a.)
The tr. pt. tor NaI.2HiO + Nal is at 64.3** and the saturated solution contains
74.4 gms. Nal jper 100 gms. (Panfiloff, 1893.)
100 gms. H^ dissolve 172.4 gms. Nal at 15® and the du of the sol. is 1.8937.
(Greenish, 1900.)
100 gms. sat. solution in HsO contain 65.5 gms. Nal at 30^. (Codieiet, 1911.)
Solubility of Sodium Iodide in Alcohols at 25*.
(Turner and Biasett, 19x3.)
100 gms. Methyl alcohol, CHi OH dissolve 90.35 gms. Nal.
Ethyl " CHiOH " 46.02
Propyl " CHtOH " 28.22
Amy! " CiHuOH " 16.30
11
i(
II
((
(I
655
SODIUM IODIDE
Solubility of Sodium Iodide in Aqueous Ethyl Alcohol at 30^
(Cocheret, 1911.)
Gms. per zoo Cms. Sat. SoL
Gms. per 100 Gms. Sat. SoL
NaL
CtHftOH.^
0UUU jTiiaso.
' Nal.
CtHftOH.
oouu raaae.
65.52
0
NaI.2B^
38. 5
53.2
MaI.sH/)
64
3.42
ti
37.49
55.37
"+Nal
54.2
18.5
u
35.65
59.24
Nal
43.8
28.5
M
33.24
61.78
u
42.35
41.7
«
30.90
68.70
fl
Data are also given for the solubiUty of mixtures of Nal + NasCOi in aqueous
ethyl alcohol at 30**.
Solubility of Sodium Iodide in Absolute Ethyl Alcohol at Temp-
eratures UP TO the Critical Point.
(TyrcT, z9zoa.)
f.
Gms. Nalper
iooGin8.CAOB
V.
Gms. Nal_per
zoo Gms. CsHiOH.
f.
Gms. Nalper
zooGm.<i.CsH^H.
10
43.77
120
45.2
240
32.7
30
44.25
160
45
250
26.2
50
44.50
180
44-3
255
21
80
45
200
42.3
260
10.8
100
45.1
220
230
•crit.
38.5
36.2
t. of solution.
261.5*
8.6
The mixtures were placed in sealed glass tubes which were heated in a specially
constructed, electrically heated air Imth. 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 Kohn, Z908.)
In CHK)H + CiHjOH. In CH,OH + CHtOH. In C,H,OH + CHtOH.
Per cent d.. of Qaa. Nal Per cent d.. of Gms, Nal Per cent j.. of Gna. Nal
CI^Hin ^V", perzooccCjHTOHia f^T. perioocc. QHtOHui ^ V^ , perzoocc.
Mnture. Sat. SoL Sat. Sol. Mixture. Sat. SoL Sat. Sol. Mirttire. Sat. Sol. Sat. Sol.
0
1.0806
35.15
0
1.3250
63.22
0
1.0806
35.15
4.37
I . 1029
37.68
II. II
I . 2853
58.45
8.1
1.0732
34.60
10.4
1.1123
38.71
23.8
1.2528
54.64
17.85
1.0720
34.05
41.02
I. 1742
45.98
65.2
I. 1387
40.71
56.6
1.0276
28.41
80.69
I . 2741
57.44
91.8
I . 0420
29.14
88.6
I. 0130
26.13
84.77
1.2886
58.92
93.75
1. 0178
26.49
91.2
I. 0104
25.88
91.25
1.3056
61.10
100
0.9968
24.11
95-2
1.0020
24.74
100
1.3250
63.22
100
0.9968
24.11
Solubility of Sodium Iodide in Several Solvents.
(At 93.5*, de Bnom, Z892; at ord. temp. Rohland, Z898; Walden, Z906.)
Solvent.
Gms. Nal
t*. perxooGma.
Solvent.
Absolute Ethyl Alcohol 22.5 43 . i
Ethyl Alcohol, du = 0.810 ord. temp. 58. 8
Absolute Methyl Alcohol 22.5 77.7
Methyl Alcohol, du ~ 0.799 o^. temp. 83 . 3
PiopylAlcohol,Ju— 0.816 ord. temp. 26.3
Solvent.
Gms. Nal per zoo cc.
Sat. Solution.
at o*. at as*.
22.09 18.43
9.09 6.23
Acetonitiile
Propionitrile
Nitro Methane o . 34 o . 48
Acetone very soluble
Furfural ... 25.10
SODIUM lODIDB
656
SOLUBIUTY OF SODIUM lODIDB IN ACBTAIODB.
(Menachtttkin. 1908.)
Giiis.per
xooGms.
GiBS.periooGiiis.
Sat. Sol.
f.
Sol.
Solid Phai^
f.
SoUdPhaM.
i4aI.aCIir
CONHi
-Nal.
^^iS^-NaL
82
BLpCofpuieicetamide CHaCX>NHt
50
S9 33
N&T.aCH|00NH|
78
95
5-32
«
60
60.S 33.9
M
74
18
10.08
It
70
62.2 34.8
M
70
25. 5
14
M
80
64.2 35.9
M
66
31.9
17.86
M
90
66.5 37.2
«l
62
37.3
20.9
If
100
69.2 38.7
M
58
41.9
23. 4*
M
1 10
72.6 40.6
W
54
46.1
25.8
If
120
78.7 44
«
50
SO
28
If
I2S
84.7 47.4
" +NaI
46
53.7
30.1
ff
ISO
8S.i 47.7
Nal
41.
S 577
32.3
f<
+NaI.aCH^CONH^
17s
85.5 47.9
M
100 oc. anhydrous hydrazine dissolve 64 gms. Nal at room temp.
(Welsh and Biodetson, 19x5.)
SODIUM lODOMEBCUEATE
A saturated solution at 24.75*^, prepared bv adding Nal and Hgli in excess to
water, contained ^.59% Na, 25% Hg, 58.25% I and 12.2% H«0, corresponding
to 0.20 mol. alkali, 0.12 mol. Hg and 0.45 mol. I. (Duboin, 1905.)
SODIUM MOLTBDATE Na.MoO«.
Solubility in Water.
(Funk, x9ooa.)
f.
O
4
6
9
10
QtoA, Mols.
Na,MoO« Na,MoO«
per zoo Gms. per zoo
Sdution. Mols. H|0.
SoUd Phase.
30.63
3383
3S.S8
38.16
39.28
3
4
4
S
S
86 Na,Mo04.zoB^
47
83
39
65 NatMoO«.aH/)
If
If
If
f.
18
32
SIS
100
Gms.
Na«MoO«
per zoo Gms.
Solution.
39.27
39- 40
39.82
41.27
4S.S7
Solid Phase.
Mols.
Na,MoO«
per zoo
Mob. HA
5 . 65 Na^oOvaHdO
5.70
5. 78
6.14
732
II
■(
i«
d of the sat. sol. at 18*^ is 1.437.
100 gms. HfO dissolve 3.878 gms. sodium trimolybdate, NaiMoiOio, at 20^, and
.7 ems. at loo^ lUnik. x869.)
13.7 gms. at loo^ lUnik, X867O
100 cc. HsO dissolve 28.^9 gms. Na1O.4MoO1.6H1O at 2 1 ^, (^ — 1 .47. (Wempe, x9is.)
Fusion-point data for KasMo04 + NaiW04 and NasMoOi + NatS04 are given
by Boeke (1907).
SODIUM NITRATE NaNOi.
Solubility in Water.
(Mulder; Berkeley, Z904; see also Ditte, X875; Maiimee, 1864; Etud, X894.)
V,
o
10
20
25
30
40
so
60
Gms. NaNQi j)er zoo Gms. Mols. pa
Solution. Water. Liter.
42.2 72.9- 73 * 6.71*
44.7 80.8- 80.5 7.16
46.7 87.5- 88 7.60
47.6 91 - 92 7.80
48.7 94.9- 96.2 8.06
50.5 102 -104.9 8.51
52.8 1X2 -114 8.97
54.9 122 -124 9.42
* Berkeley. T ^t 1x9*.
f.
80
100
120
180
220
22s
3i3t
Gms. NaNC\ per zoo Gms.
Solution. Water.
59. 7 148 -148. *
64.3 180 -I7S-8
68.6 218 -208. 8t
78.1 3S6.7
83- 5 S06
91.5 1076
100 00
tin.pt.
Mob. per
Liter.
10.35*
11.30
I2.22t
657
SODIUM NITR4TE
Solubility of Sodium Nitrate in Aqueous Ammonia Solutions at 15*".
(Fedotieff And Koltunoff, 1914.)
In Aqueous NH|.
Sat.SoL
1.253
1.233
I. 212
Gms. per xoo Gms. H9O.
NH«.
13.87
17.28
20.38
NaNOb.
75.03
73.99
73.18
In Aqueous NH, + NH4NO,.
Sat. Sol.
1.324
1.330
Gms. per xoo Gms. H9O.
NH«.
12.91
16.97
NHtNGi.
83.51
128.9
NaNOb.
74.10
69.40
Solubility of Sodium Nitrate in Aqueous Solutions of Nitric Acid at o^
(Engel, Z887; see also Schults, x86o.)
rater
Its per
10 cc. Sc
tutioa.
0..
Sp. Gr. of
Soludoos.
Grams per
xoo cc. bolat
NaNOa.
HN
NaNOt.
HNOa:
66.4
0
I.34X
56.5
0.00
63
7
2-65
I 338
54-2
1.67
60
•S
5
•7
I 331
51.48
3-59
S6
9
8
8
1.324
48.42
5-55
52
•75
13
57
1.312
44.88
7.92
48
•7
16.
9
1.308
41.44
10.65
39
•S
37
0
1. 291
33-61
17.02
35
.1
3*
25
1.285
29.86
20. 33
31
.1
37
25
1.282
26.46
23.48
23
•5
48
.0
1.276
20.0
30.26
18.
0
57
25
1.276
15-32
36.09
13.
9
71
0
Z.29I
10.97
44.76
Solubility of Mixtures of Sodium Nitrate and Potassium Nitrate
in Water at 20®.
« . . (Caznelly and Tbomsoii, x888.)
Feromt
NaNOain
Miztuxes
Gms.
per xoc
HsO.
>Gms.
Per cent
NaNOsin
Mixtures
Used.
Gms.
per xoc
Hip,
> Gms.
Used.
KaNOa.
KNOs.'
KaNOa.
KNOj.
100
86.8
0
45-7
53-3
34.7
90
96.4
13-2
40
45-6
35-5
80
98.0
38.5
20
20.8
33-3
60
90.0
47.6
10
9 4
31-5
SO
66.0
40.0
0
0.0
33-6
too gma. HiO dissolve 24.9 gms. NaCl + 53.6 gms. NaNOi at 20**.
CRttdorff, X873; Karsten; Nicd, xSgx.)
Solubility of Sodium
lifiUigram Mols. per xo
cc. Solution.
l^asO.
NaNOftJ
CO
66.4
2.87s
62.5
6.1
57 15
".75
47-5
a6.o
29 -5
39 0
17-5
45.88
13 19
60.88
6.0?
Nitrate in Aqueous
Hydroxide at o**.
CEngel, X89X.)
Sp. Gr.
of
Solutions.
Solutions of Sodium
Gruns tter xoo cc.
Solution.
KaOH.
I
I
1
I
I
I
1
I
341
338
333
327
326
332
35^
401
o
2
4
10
20
31
36
48
o
30
89
21
83
25
76
75
NaNOi.
56 50
53
48
40
25
14
II
5
19
63
43
10
89
33
15
SODIUM NITRATE
658
Data for equilibrium in the system sodium nitrate, sodium sulfate and
10", 20^ 25% 30', 34® and 35** are given by Massink (1916, 1917).
water at
SoLUBiLiry OP Sodium Nitratb in Aqueous Scx^utions of Sodium
Thiosulfatb.
(Kienuum uid Rodrmiind, 19x4.)
Results at 9^
Results at 25^
Cms. Der xoo Cms.
S«t..Sol. Solid Phue.
Gms. per
xoo Cms.
Sol.
•
Solid Phaie.
NaNOfe. Na,SA.
NaNOb.
NaAQi.
33.31 12.26 NaNC^
35-42
12.72
NaNOb
22-57 23.41 " +NitSA.5H.O
25.40
24.25
u
4.22 34.77 NitSA.5^
19.90
31-81
" +NaA<VsW>
18.02
32.83
Na.SA.sHiO
4.33
40.50
M
Solubility of Sodium Nitratb in Alcohols.
100 gms, abs. methyl alcohol dissolve 0.41 gm, NaNOi at 25®.
100 gms. abs. ethyl alcohol dissolve 0.036 gm. NaNOi at 25^.
(de Bnqm, x89s.)
Scx^ubilitt of Sodium Nitratb in Aqubous Ethyl Alcohch« at
Differbnt Tbmferaturbs.
(Bodlliider, 1891; Taylor, 1897; Bathrick, 1896.)
Res
nilts at 13** (B.).
Results at 16.5*" (B.).
Sp.Gr.of
Gms. per xoo cc. Solution.
Sp.Gr.oC
Solutions.
Gms. per
xoo cc. Solution.
Sofodons. i
[leH^H. H9O.
NaNOs.
CsHsOH.
HsO. NaNOs.
1.3700
00 75.34
61.66
1-3745
00
75.25 62.20
1-3395
308 73-53
57-34
1.3162
6.16
70.82 54 64
1.3120
6.01 71.81
53-39
1.2576
11.60
68.10 46.06
1.2845
8.30 70.85
49-30
I. 2140
16.49
65 04 39-87
1.2580
10.91 69.47
45-42
1-1615
22.17
61.67 32.31
1-2325
13.77 67.12
42.36
I 0855
32.22
52.92 23.41
I. 2010
16.46 66.16
37 48
I .0558
37-23
48.50 19.85
1.0050
43-98
42.78 13.74
0.9420
52.60
32.13 9.47
0.9030
60.00
25-65 4-65
0.8610
63.16
21.31 1.63
Results at 30* (T.).
Results at 40^ (Bathrick).
Wt. per cent Gms. NaJJOj
Wl
t.
Gms. NaNOt
Alcohol in Pcr xoo
ums.
te cent
Alcohol.
per xoo Gma.
Aq. AloohoL
Solvent. SolatioQ.
Water-
0
49.10
9^-45
0
104.5
5
46.41
91-15
8.
22
90.8
xo
43-50
85-55
17.4
73-3
20
37-42
74-75
26.
0
61.6
30
31-31
65.10
36.
0
48.4
40
25.14
55-95
42
8
40.6
50
18.94
46.75
55-3
27.1
60
12.97
37-25
65
I
18. 1
70
7.81
28.25
77-
0
9.4
90
1. 21
12.25
87
.2
4.2
659
SODIUM NITR4TE
Solubility of Sodium Nitrate in Aqueous Alcohol at 25^
(AnnstxoDg and Eyie, 1910-ix.)
Solvent.
Mob. QHsOH . Gms. &H«0H
per 1000 Gms. Bfi, per xooo Gms. BiQ.
O
0.25
0.50
I
2
O
11.51
23 03
46.06
92.12
Gms.NaN0b
per 100 Gms.
Sat.SoL
47-93
47.32
46.73
45.43
43.04
Solubility of Sodium Nitrate in
Results at 30^
(Tayloc X897.)
Aqueous Solutions of Acetone.
Results at 40**.
(Batbikk, 1896.)
Wt. percent
Acetone in
Solvent.
Gms. NaNOi
per 100 Gms.
Scdution.
O
5
9
20
30
40
50
60
70
80
00
09
49.10
46.96
45'"
40.10
35 08
29.80.
24 -34
18 -55
13 IS
7.10
1.08
Water.
9^-45
93
90
83
77
70
64
59
50
38
20
20
40
70
20
75
40
95
50
20
20
Wt.
percent
Acetone.
Gms. NaNOi
per zoo Cms.
Aq. Acetone.
0.0
8.47
16.8
25.2
91.3
78-3
66.4
34-3
44.1
57-9
46.3
53-9
64.8
76.0
87.6
32-8
23-0
10.8
3-2
100 gms. hydroxylamine dissolve 13. i gms. NaNOs at 17-18^ (de Bniyn, 1892.)
100 cc. anhydrous hydrazine dissolve 100 gms. NaNOt at room temp.
(Welsh and BroaerBon, XQ15.}
Fusion-point data for NaNOt + NaNOi are given by Bruni and Meneghini
(1909, 1910).
Results for NaNOj + SrNO« + KNOi are given by Harkins and Clark (1915)
and results for NaNOt + TlNOt by van Eyk (1905).
SODIUM Nrram NaNO,.
Solubility in Water.
(Oswald, xgxa, 19x4.)
f.
Gms. NaNOi per
zoo Gms. Sat. Sol
Solid Phase.
•
f.
Gm-NaNO,
100 Gnu. Sit.
id.
SolMPhan.
- 4.5
9.1
Ice
30
47.8
NaNOk
- 9
23.8
«
40
49.6
ff
-12.5
29.6
M
52.5
SI -4
M
-15.5
Eutec. 39.7
" +NaNQi
65
54-6
<•
- 8 .
40.8
NaNQi
81
57-9
M
0
41.9
It
92
S9-7
M
10
43.8
M
103
63.6
M
20
45-8 (i-
I4S8S) "
128
68.7
U
100 gms.
HiO dissolve 83.^
( gaa. NaNOi at i
>5\
(Diven, 1899.)
100 gms. H|0 dissolve 83.25 gms. NaNOi at 1$^.
(v. Niementowski and v. Roszkowski, 1897.)
100 gms. HiO dissolve 73.5 gms. NaNO« at 15**, du - 13476.
((Greenish and Smith, 1901.)
N*N(V
NkNCV
73
0
68
19
67
363^
64.9
41. ?•
50.3
46.8
302
S5-4
0
74.2
SODIUM NITBm 660
Solubility of Sodium Nitrite in Aqueous Solutions of Sodium
Nitrate and Vice Versa at Several Temperatures.
(Oswald, 1912, 19x4.)
Results at o^ Results at 31*". Results at 52^ Results at 103^
Gma. per xoo Gms. "Bfi. Cms, per icp Gms. KJO. Gms. per 100 Cms. HiO. Cms, per loo Gms. KJO,
NaNOb. NaNCV NaNOb. NaNQ^ NaNQ,. NaNO^.
84.75 o 108.8 O 166 O
81. 1 9.6 104.3 20.6 153.3 33.2
79-7 23.5 99.5 43.2 148.8 58.8
73.8 50.8 98.8 82 * 142.4 116 *
73.1 54-5* 65.2 88 100 126.8
64.2 56.7 44.2 92.9 60.1 142.9
46.8 62.8 27.2 101.4 o 181. 2
21.6 74.7 14.7 109
o 89.3 o 118
* Both salts in solid phase.
Similar results are also given for 18", 65®, 81® and 92*.
100 gms. HfO, simultaneously saturated with both salts, contain 53.9 gms.
NaNOi + 11.8 gms. NasS04 at I6^ (Oswald, 1914)
Solubility of Mixtures of Sodium Nitrite and Silver Nitrite in Water
AT 14^ and at 22®. (See also p. 620.)
(Oswald, 19x3, 19x4.)
Results at 14^. Results at 22^
Gnu. pa xoo Gms. H|0. Gms. per zoo Cms. H9O. » ,. . «. . ^ . r^
^TTTTT- — • A vt!v ^t-zttt- — * z-dS* Solid Phase m Each Case.
NaNO^. AgNC>|. NaNOi. AgNOb-
55 15.2 58.3 21.5 AgN0b+Na,A&(N0»)4Ja/)
74-7 11.3 78.3 13.4 NaN0,+Ns.Ag,(N0,)4.H^
100 gms. abs. methyl alcohol dissolve 4.43 gms. NaNOs at i9-5^-
100 gms. abs. ethyl alcohol dissolve 0.31 gm. NaNOs at 19.5 • (de Bruyn, 1892.)
SODIUM BHODONITBm Na«Rh,(N02)is.
i(X) gms. HsO dissolve 40 gms. at 17^, and 100 gms. at 100^. (Leidie, 1890.)
SODIUM OLEATE C8Hi7CH:CH(CHi)7C(X)Na.
Solubility in Water and Aqueous Bile Salts.
(Moore, Wilson and Hutchinson, 1909.)
c^i.,^^4. Gms. Oleate per
So»v«*t- 100 Gms. Sat. SoL
Water 5
Aq. 5% Bile Salts 7.6
Aq. 5% Bile Salts + 1% Lecithin 11 .6
SODIUM OXALATE NasCiO«.
Solubility in Water.
(Souchay and Leussen, 1856; Pohl, 1852.)
t*. IS-S*. ai'S*. ^ too*.
Gms. Na«C804 per loo gms. H2O 3.22 3 . 74 6 .33
100 gms. sat. solution of sodium oxalate in water contain 3.09 gms. NasCi04 at
15** and 4.28 gms. at ^o**. (C>>Iam, 19x6.)
100 gms. 95% formic acid dissolve 8.8 gms. NatQlOi at 19.3^ (Aschan, 19x3.)
66i
SODIUM OXALATE
SODIUM OXALATE
Solubility of Mixtures of Sodium Oxalate and Oxalic Acid in
Water at 25®. (Footc and Andrew, 1905.)
Gms. per xoo Cms.
Solution.
Mols. per xoo Mols.
Solid
Phase.
rtaC|04. NaiCsO*.
HaCsO*.
NasCsO«.
I0>20 ...
2.274
• • •
HsC«04.3HsO
10.50 0.83
2.370
0.130
" H^sO«.3H3O+HNaC«O«.H«0
9.15 0.71
2.032
0.106'
6.SS 0.86
1-493
0.125
_ ^ ^_ ^
Doable Salt. UNaCsOt.H«0
1. 14 1.25
0.234
0.172
0.47 3 -20
0.098
0.446^
0.42 3.85
0.090
0.541
HNaC«04.HaO + Na«C|0«
3.60
• • •
0.502
NaaC30«
Solubiuty of Mixtures of Sodium Oxalate and Other Sodium Salts
IN Water at 15** and at 50**. (Colani, 1916.)
Gms. per xoo Cms. Sat. Solution. c^H j p^^^^
IS
SO
IS
SO
IS
so
0.027 Na2C204 + 26. 28 NaCl
0.063 " +26.64 "
+ 10. 26 Na2S04
+ 31.95 "
+ 45.86 NaNOa
+ 5306
0.86
0.22
0.051
0.047
u
((
Na«Q04+Naa
Na«C,04+Na,SO4.xoH^
" +Na«S04
Na,Q04+NaN0b
Equilibrium in the System Sodium Oxalate, Uranyl Oxalate and
Water at 15** and 50**. (Coiani, 19x7.)
Cms.
Results at 15®.
xoo Cms.
,t. Sol.
Ka,C,04. UOjCA.
3.09 O
4.93 3- 14
1.80' 5.01
0.80 2.65
O 0.47 U0,C,O4.3H^
Solid Phase.
Na,Q04
3.X.2.5+24.5.IZ
2.4.5.11 +U0|Q04.3H^
SoUd Phase.
Results at 50".
Gms. per zoo Gms.
Sat. Sol.
Na«C^4. UO,C,04.
4-28 O Na,C,04
9.03 13.09 " +a.i.2.s
4.62 12.33 a.x.3.s +2.2.3.S
3.60 9.84 2.2.3.S+24.S.XI
1. 01 3.58 a4.SM+U0»C,04.3Hi0
O I UOs.QO4.3HsO
2.1.2.5 = Nai(UO,)(C,04),.5H,0, 2.2.3.5 = Nas(UO,),(C,04)i.5H20, 2.4.5.11 =
Na,(UOi)4.(C204)».iiH,0.
SODIUM PALMITATE CHs(CHt)i4C00Na.
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.
100 gms. sat. solution in 5% aq. bile salts + 1% lecithin contain 2.4 gms.
sodium palmitate. (Mooie, Wilson and Hutchinson, X909.)
Solubility of Sodium Palmitate in
Palmitic Acid. (Donnan and white, xgxi.)
Gms.
Na Pafanitate
per xoo Gms.
Liquid Phase
Gms. Na Palmitate
Gms.
Na Pahnitate
per xoo Gms.
Liquid Phase.
Gms. Na Palmitate
f.
per xoo Gms.
Solid Phase (Na
PahniUtc+
Palmitic Add).
r.
per 100 Gms.
Solid Phase (Na
PahniUtc+
Palmitic Acid).
60.2
2.3
0.7
71
22.60
25.38
62
4.96
II. 12
72.9
28.65
35.05
64.4
7.98
13.78
73. s
29.07
35- 23
66.65
12.28
16.36
76
30.7
35.9
67.7s
13.72
18.70
79.2
33.36
35.66
68.95
15.56
2^.55
82
36.02
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 PBENOLATE
662
SODIUM p NITBOPHINOL C<H4.0Na(i).NOs(4).
Solubility in Water and in Aqueous Normal Solutions of Non-
Electrolytes.
(Gokbchmidt, 1895.)
Gms. CA-ONad) J«fOi(4) per 100 Gms. Solntkn in:
a3-7
38.6
30.6
35-9
36.1
40.3
45-2
SO. I
Water.
5-597
6.721
7.256
8.125
8.851
8.883
9.881
"•^35
12.730
Alcohol.
5-615
6.874
Urea.
6.244
7.489
GWoerine. Acetooe. Propioiutril. AcetonitrU. Urethane.
6.188 6.225 6.257 6.065 6.520
7-571
7.440 7.498
8.318 9.000 9.025 9.025 9.066
7.328
8.886
7.889
...
9-507
9.683 9.688 9.665 9. 911 9.667 10.248
10.147 10.666 10.777 10.695 10.905 10. 667 11.379
II. 513 12.068 12.229 ... ... ... 12.869
13.133 13555 13.785
The soHd phase is CJl4ONa.Nd1.4H1O below 36% and Cai4ONa.NOk.2H1O
above 36** in each case.
SODIUM PHOSPHATE (Ortho) Na,P04.i2HiO.
Solubility in Water.
(Mulder).
■
0
10
Gms. per zoo
Gms. HA
1-5
4.1
r.
25
30
Gms. per zoo
Gms.E^.
15.5
20
60
80
Gms. per 100
Gms.ByO.
55
81
20
II
40
31
too
108
50
43
SODIUM Hydrogen PHOSPHATE NaiHP04.i2HiO.
f.
— 0.43
— 0.24
— o.5£utec
+0.05
10. 26
I5-"
20
25
30.21
30.76
32
33-04
34
35.2 tr.pt.
36.4s
37.27
39.2
tt
Gms. Na|HP04
per xooGms.
Solubility in Water.
(Shiomi, 1908; Menaes and Humphrqr> zgzi.)
Gms.NaJIPO|
t*. periooGms. Solid
45 67.3 Ni,HF0«.7H^
47.23 76.58(8)
48 . 3 tr. pt. ... J NatHPO«.7HriO+
40 • • •
Sdid Phase.
1 . 42 Ice
0.70
" +Na.HP04.MHiO
1 . 67 Na|HP04.Z3H^
3 .55(5)
S-23(S)
7.66
12
20.81 (S)
23-41(8)
25-7
30.88 (S)
33-8
«
M
M
II
M
II
M
U
II
... (S)
47Si(S)
SI. 8
II
II
+Na,HP04.7B^
•i
Na|HPO«.7H/)
II
50
55-17
60
70.26
80
89.74
90.2
95 tr.pt.
95.2 ••
96.2
99.77
105
120
... (S) 1 Na,HP04.sHiO
80. 2 NstHPOi-sHdO
81.4 (S)
82.9
88.ii(S)
92.4
102.87(8)
lOI.I
II
II
II
M
... (S)
104.6
102.15(8)
103.3
99.2
II
« +Na«HFQ«
« u
Na,HFO«
M
Results marked (S) by Shiomi, all others by Menzies and Humphrey.
100 gms. HiO dissolve 12.2 gms. Na2HP04 at 25*^, determined by refractometer.
(Osaka, zgoj^.)
1 00 gms. HiO dissolve 5.23 gms. NaiH PO4 at 1 5^ du « 1 .049. (Greenish and Sm^ 190K .)
100 gms. alcohol of du ■» 0.941 dissolve 0.33 gm. NaiHPOi at 15.5^
663
SODIUM Dihydrogen PHOSPHATE NaHsPO«.
Solubility in Water.
Gmadwi, Z911-X2.)
SODIUM PHOSPHATES
Giitt.NaHJ^
Gna.'StB^PO,
V,
per xooGina.
SdidPluM.
f.
H«0.
Solid Phaae.
O.I
57.86
NaHO^aB^
45
148.20
NaH»PO«.fV)
5
63.82
(1
SO
158.61
M
10
69.87
M
55
170.85
«
IS
76.72
CI
57
175.81
M
20
85.21
M
S7-4«i
• pc. • ■ •
" +NaHaOi
25
94.63
W
60
179.33
NaH»PQ«
30
106.45
«
65-
184.99
M
35
120.44
«I
69
190.24
M
40
138.16
M
80
207.29
M
40.81
tr. pt. . . .
" +N*^F(VIV>
90
225.31
M
41
142.5s
NiB|P04.B^
99.1
246 . 56
M
SODIUM Acid PHOSPHATE NaHsP04.H,P0«.
Solubility in Water and in Anhydrous Phosphoric Acid, Dbtbrminbd
BY THE Synthetic Method.
(Pamvano and Mieli, 1908.)
Solubility in Water.
Solubility in HtPOi.
Gms.
■Gms.
Gms.
NaHfOi- NaK.P04.-
t*. ^^per Solid Phase. V. EbPO«per
xoo Oms. zoo Gms.
Solid Phase.
NaHiPOiw-
V, l£p&«per
100 Urns.
Sat.SoL
Sat.SoL
SaLSoL
- 57 20.77
Ice
79.7 87.48
NaHa*04
98. s S2.72
— 7.9 26.92
u
85 88.65
i<
III 69.59
-II. 4 34.15
M
IOI.7 91.47
"+NaH,P04.H,P04
"9 77. SS
-38 56.66
M
104.5 92.67
NaHa*0|.H|P04
122 81.71
—34 80.46 NaHiPO, HO 95.79
M
123 87.20
41 81.82
SI. 7 83-68
M
W
119 97.99
126.5 100
U
,, m. pt. of the H1PO4 -i 40.6*
Data are also given for the fusion points of NaHsPOi + H1PO4.
Fuaon-point data
for mixtures of NaPOi + Na4Ps04 are given by Parravano
and Calcagni (1908,
1910.)
Equiubrium in tuk
System Sodium Hydroxidb,
Phosphoric Acid and
Water at 25*.
(D'Ans and Schreiner, xgxoa.)
Mob. per 1000 Gms. Sol.
^olid Pluuv
Mols. per xppo Gms. Sol. ;..,,, „^ __
Na. PO4.
Na.
PO4.
— • w«Mwi A uaaiM
13.32
Na0H.H/)
6.76
4.88
Na«HP04.7H^
4.28 0.040
Na«P04.Z9B^
7.31
S'55
" unstable
3.24 0.183
M
6.76
4.88
" +NBtHP04.aH^
2.24 0.752
<C
6.19
4.68
NaflHPQ4.9B^
2.73 1.08
«
6.0I
4.67
u
3.48 1.33 Na«P04.iaH/)+Na,HP04.iaH^
S.I2
4.36
II
3.62 Z.09
Na«UPO|.Z2HdO
4.81
4.22
a
1.56 0.78
M
4.36
4.08
M
2.38 1.60
M
4.06
4.03
M
3.18 2.24
M
4.19
4.38
M
4.65 3.55
«
4.32
4.96
M
5-63 3.87
W
4.65
S.89
M
6.31 4.63
Na,HP04.7H^
4.88
6.40
M
SODIUM PHOSPHATES 664
SODIUM PyroPHOSPHATE Na4P«Oy.ioH«0.
SoLUBiLiry IN Watbk.
(Mulder: Poggiale.)
f.
Gms. per
tf
f.
Gms. per
xoo Gma. ByO.
V •
xoo Gms. H^.
100 Gms. H^.
0
3.16
25
8.14
60
21.83
10
3-95
30
9.9s
80
30.04
20
6.23
40
50
13.50
17.45
100
40.26
SODIUM PyroPHOSPHATES.
Solubility in Water.
(Girsn, x9Q3a.)
Gms. Anhydxoos Salt
perioo oc ScUj^ SoL
62.7
14. 95
28.17
SODIUM PHOSPHITES
Solubility of Sodium Phosphitbs, siCn in Water.
Gms. Salt
Salt. Fonnola. t°. per 100 Gms. Aixthocity.
HtO.
Hydrogen Phosphite (NaH)HP0,.2lH,0 o 56 I (Amat.— Compt.
Salt.
FannQia*
f.
Monosodium Pyrophosphate
Disodium Pyrophosphate
Trisodiuia Pyrophosphate
NaH.PiOr
NaiHiPiOr.6HiO
Na«iiPA.6H,0
18
18
18
U It
10 66 ) nod. xo^ X35X. '8&I
42 193
Hypophosphate Na^PtOc-ioHjO cold 3.3 )
Hydrogen Hypophosphate NaJHP,0,.9H,0 ? 4. 5 [ ^Ti??% j
Tri Hydrogen " NaH,P,Oe3H,0 cold 6.7) ^im. axi. x. -8.^
Di Hydrogen " Na,H»P,0,.6H,0 cold 2.2 | (sd«r-Ltehiir'a
Di Hydrc^ " Na,HJP,0«.6H,0 b. pt 20.0 J Ami. 187, 33x7^77^
Hypophosphite (NaH)HPO,.H,0 25 100. o | (U.S. P.)
Hypophosphite (NaH)HPO,.H,0 b. pt. 830 J
100 gms. H^ dissolve 108.7 gnis. anhydrous sodium hypophosphite (NaHsPOO
at 15% du of sat. SoL.a 1.388. _ (Greenish and Smith, xgoxO
SODIUM (Double) PHOSPHATE, FLUORIDE Na«P04.NaF.i2HsO.
100 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. (Bxiegleb. 18560
SODIUM PICBATE CeHt(Na)t.ONa.H,0.
Solubility in Water and in Aqueous Solutions at 25*.
(Fisher and Mllosxewski, i9xo<)
100 cc. HiO dissolve 4.247 gms. C6Hs(NOt)s.ONa.HsO at 25^
Solubility in Aq. ^"^ CtH^(NO^t'ON*J<0 per 100 cc Aq. Solution of NonnaKty:
Solution of: ' -- ^
*'*" " ^" 0.01. o.oa. 0.04. 0.066. 0.X0. 0.25. 0.5. I.
NasCOs 4- 159 4.044 3.807 3.434 3.187 2.017 1. 120 0.611
NaCl 4.189 3.956 3.677 3-335 3-02i 1.678 0.846 0.410
Na2S04 4.246 4.162 3.879 3.651 3-I9S 2.053 1.156 0.552
Na«P04 4-235 4.051 3-8x4 3S62 3-225 2.219 1329 0.705
NaOH 4.192 4.048 3.715 3.339 2.941 1. 781 0.921 0.371
NaNOs 4.154 4.029 3.710 3.363 3.041 1.932 0.943 0.684
NaBr 4-190 4. 117 3.770 3.384 3.024 1.777 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).
665 SODIUM SALICYLATE
SODIUM SALICYLATE C6H4.0H.COONa.
Solubility in Aqueous Ethyl Alcohol at 25^ (Seidell, 1909, 1910.)
Vt Per cent
Sat.SoI.
Gms. CeHiQH-
Wt. Per cent
duoi
Sat. Sol.
Gms. CeHiGH-
SoTvent.
COONa i)er loo
GnM. Sat. SoL
QILOHin
Solvent.
COONa per loo
Gms. Sat. Sol.
0
1.256
53 56
60
1.066
38.40
10
1.235
52.10
70
1. 016
33
30
1.205
50.20
80
0.957
25
30
1. 176
48
90
0.885
15
40
1. 142
45 50
92.3
0.864
12
50
1. 106
42.20
100
0.805
3.82
100 gms. sat. solution in water contain 51.8 gms. C8H40HCOONa 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. CeH40HCCX)Na at ord. temp.
(Schlami), 1894.)
Sodium salicylate distributes itself between olive oil and water at 15^ in the
ratio of 0.156 gm. C6H40HC(X)Na per 100 cc. oil layer and 1.444 gins, per 100 cc.
aqueous layer. CHanaas, 1903.)
SODIUM SELENATE NasSe04.ioH20.
Solubiuty in Water. (Funk, sgooa.)
Gms. Mols. Gms. Mols.
Solid
Phaaeb
Na^Sc04
40 NaiSeOti per
' xoo Gms.
Na9Se04jper
zoo Mob.
Solid
Phase.
%•
NaaSeOi per NasSe04per
zoo Gms. zoo Mols.
Solution.
HaO.
Sdution. HsO.
0 11-74
1.26
Ns»SeQt.io^O
35-2
4S-47 7-94
IS 25 .01
318
M
39 S
4S.26 7.87
18 29.00
3 90
M
SO
44.49 7 63
25 •» 36 91
SS7
m
7S
42.83 7.14
27 39.18
6.13
m
100
42.14 6.93
30 44.05
7 -so
M
Sp. Gr. of saturated solution at 18° — 1.315*
SODIUM [SILICATE NasSiO,.9HtO.
Solubility in Aqueous Sodium Hydroxidb and Sodium Chloridb
Solutions. (Vesterbag, 1912.)
Gms. per zoo cc. Sat. Solution.
Solvent. t*. dn of f * \
Sat. Sol. NaiO. SiO^ - Na,Si0|.9H,0. NaQ.
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 i . 258 4. 563 4. 376 20. 64 27 . 91
Solid phase NasSiOs.9HiO in each case.
Fusion-point data for NajSiOa + SrSiOj are given by Wallace (1909). Results
for Na^i6t + NajWO* are given by van Klooster (1910-11).
SODIUM STAGNATE Na,SnO,.3H,0.
100 gms. H2O dissolve 67.4 gms. at o^, and 61.3 gms. at 20^ Sp. Gr. of solution
at O® = 1.472; at 20° = 1.438. (Ordway, 1865.)
SODIUM SUCCINATE (CHt)t(COONa),.6H20.
Solubility in Water. (Marshall and«*ain, 1910.)
Gms. (CH,)r
(COONa), s^ p^^
per xoo Gms. ^^ ™^'
H,0.
56 . 3 (CH,),(CX)0Na),.6H/)
78.49
83.38 " +(CH.),(COONa),
86.63 (CHt),(COONa),
Gms. (CHs)r
^ , ((X)ONaT,
* [per xoo Gms.
Solid Phase.
f.
Bfi.
0 21.45
(CH,),(C00Na)a.6H,0
50
12. S 27.38
«
62.5
25 34.90
It
64.9
37. s 43.64
ii
75
SODIUM SUCCINATES
666
Solubility of Sodium Hydrogen Suconatb in Water.
(Biinhall and Bain, 19x0.)
f.
Gfltt. (ClUr
(C00H)(CGONa) Solid Phaae.
I)er zoo Gma. H^.
Giiia.(CEUt-
«*. (COOB)(pSom Solid Phaae.
per zoo Gms. HflO.
o
1 7.55 NaHSu*.3H^
38.7 63 . 99 NaHSu.3H«0+NaHSa
2.5
27.93
SO 67.37 NaHSu
2S
39 82
^^'S 76.15
37. S
60.01
75 86
Equiubsiuii in the System Sodium Succinate, Succinic Acid and Watbr.
(Manhall and Bain, z9zo.)
Results at o^
Results at
25*.
Gni8.per
zoo Gms.
Gms. per xoo Gms.
Sat. Sol.
Sol.
Solid Phase.
Solid Phase.
Na«Su.
HiSu.
'Na«Sa.
H«Su.^
0
2.68
H«Su*
0
7.71 ]
H«Sa
3-23
4.76
((
3.68
10.26
<i
S.38
5 83
u
8,99
13.35
«
8.27
7.12
" +NaHSu.3H^
12.64
15-53
«
8.67
6.27
NaHSu-aHgO
15.26
16.90
" +NaHSu.3HdO
9.68
4.74
(1
15.97
13.83 NaHStt.3HiO
11.74
3.49
tt
18.89
8.41
II
15.62
2.34
fi
22.71
5.65
i«
18.36
1.90
" +Na,Su.6H/>
26.88
4.08
" +Na«Su.6HdO
18.07
1.67
Na«Su.6H^
26.50
2.38
Na«Su.6HdO
17.87
0.94
M
26.11
0.85
«
17.64
...
25.87
0
II
Results at 50**.
Results at
75'.
0
19.27
H«Su*
0
37.64
B^
595
22.90
t<
8.22
40.38
U
1025
25.33
(1
13.14
42.50
M
15-49
28.-73
It
16.93
44.38
<l
19.65
31.73
" +NaHSu
19.56
45.98
" +NaHS«
20.72
26.51
NaHSu
21.88
35.60
NaHStt
22.53
18.44
(1
24.30
26.82
II
25. 53
13.09
II
29.45
15.28
II
28.28
9.46
M
36.11
7.79
. "
30.48
7.38
II
41.26
4.93
II .
37.33
4.20
" +Na,Su.6H,0
45 27
4
" +Na.Su.H/)
36.85
3.88
Na«Stt.6H,0
45.36
3.17
Na.Su.H«0
36.67
2.66
II
45-93
1.23
II
36.43
0
M
46.42
0
\
The following double and triple points
were located:
t*
Gms. per zoo Gms. Sat. Sol.
^n\{A Pt^-- >
% .
Na,Su. HsSu.
OOllU IT
34.9
30.8 5.6
NaHSu.3H^+NaHSa+Na.S«.6H^
37.8
19.6 25.46
NaHSa.3H^+NaHSu+H«Sa
38.7
22.47 16.44
NaHSu.3H^+NaHSa
63.4
42.92 3.64
Na,Sa.6H^+Na«Si
i.H^+NaHSa
64.9
45-43
Na«Sa.6H«0+Ka,Si
ii.H|0
*In the above tables the abbreviation Su is used for (CH2)s(C00)s.
667
SODIUM SULFATE
SODIUM SULFATE NaiS04.
Solubility in Water.
(Mulder; Lflwd, 1851; TUden and Shenstooe, 1883'; Etard, 1894; Funk, xqooa; Beikdey, 1904.)
*•• ^
Gms. Na^504 per MoIs.
looGma. NasSOkDer
Solid
Phase.
**^
Gms. Na^S04 per
100 Gms.
Soludoo. Water:
Mola
^Ia>S04
Uteri
'• Solid
^
Solution.
Water. Liter (B.).
0
4.76
5.0 0.31 NaaSQ*.!
coHsO
• 50
31 -8
46.7
2.92 Na^O«
s
6.0
6.4 ...
u
60
31.2
45-3
2.83 ••
10
8.3
9.0 0.631
M
80
30.4
43-7
2.69 •
IS
II. 8
13.4 ...
M
100
29.8
42 5
2.60
30
16.3
19.4 1.32
M
120
29s
41.9s
M
25
21.9
28.0
M
140
29.6
42
M
a7S
25.6
34.0
M
160
307
44.25
M
30
29.0
40.8 2.63
«
230
317
46.4
M
31
30.6
44'0
M
0
16.3
19 S
Na^SQ..7B^
32
32 -3
47.8
•
19.4
24
H
32.7s 33'^
50.65 3. II
H
10
23.1
30
••
33
33 0
50.6 ... Na^SOft
IS
27.0
37
•1
35
33-4
50.2
U
30
30.6
44
M
40
32-8
48.8 3.01
m
as
•
34-6
S3
«
The
very carefully determined values of Berkeley are as follows:
Gms.
Gms.
f.
JgOf
Sat. Sol.
^^iS^SoBd Phase.
r.
JgOf
Sat. Sol.
N8,S04P«
xoo Gms.
Sdid Phase.
H«0.
H,0.
0.70
1.0432
4.71 Na,SO«.i
oHiO
32.
5tr.pt.
• • •
Na,S04
.ioH,0+Na«SQ«
10.25
1.0802
9.21 "
33-
5
I ■ 3307
49-39
Na,S04
15.65
1.1150
14.07
38.
15
1.3229
48.47
ft
20.35
I. 1546
...
44.
8s
I. 3136
47.49
(1
24.90
1.2067
27.67
60.
10
I. 2918
45.22
i<
27.6s
I . 2459
34.05
75.05
1.2728
43. 59
« M
30.20
I . 2894
41.78
89.
9*
1.2571
42.67
M
31.95
1.3230
47.98
lOI.
I . 2450
42.18
M
• B.
pt.
.
The following additional data at high temperatures, determined by the sealed
tube method, are given by Wuite (1913-14).
f.
Mol.
N8,S04.
Gms.
Na,S04per
xoo Gms.
H«0.
Solid Phase.
f.
Mol.
Per cent
NaiSOf.
Gms.
Na|S04per
xoo Gms.
Solid Phase.
62
5.39
44.92
NatSOf (rhombic)
208
5-39
44.92
^f a«S04 (rhombic)
70
5.27
43.87
II II
235 t
tr.pt.'
• • •
" +monodinlo
80
5.18
43.07
II 11
241
5.39
44.92
NaiSO« (monodinic)
120
5.04
41.84
If If
250
5.04
41.84
U If
190
5.25s
43.74
II If
279
4.12
33.84
II f«
192
S.27
43.87
i( If
319
2.56
20.71
M It
Supersolubilitv curves for the ice phase, NatS04.7HtO phase and NaiS04 phase
were determined by Hartley, Jones and Hutchinson (1908) by ap^tating mixtures
of sodium sulfate and water contained in sealed tubes, and noting the points at
which spontaneous crystallization occurred while the tubes were gradual^ cooled.
The effect of mechanical friction, produced by bits of glass, garnet, etc., was also
studied.
SODIUM SULFATE 668
SODIUM SULFATE
Solubility of Mixtures op Sodium Sulfate and Magnesium Sulfatb
IN Water (Astrakanite) NasMg(S04)i.4H«0.
(Roonboom, 1887, z888.)
Hob.
per 100
Grams
per zoo
••.
Mob.,HsO.
Granu
NajSO«.
iHiO.
^>sSO«.
MgSO«.
MgSO«:
33
2-95
4.70
23 -3
31 4
94 S
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
33
2-95
4
70
23
3
31-4
34 S
3-45
3
62
27.
2
24.2
30
458
2.
91
36.
I
19. 1
35
4-3
2.
76
33'
9
18.44
18.5
3 41
4
27
43-
0
45 S
33
2.8s
4-
63
35-
2
48.9
245
3.68
4
76
33-
S
50 -3
30
2-3
S-
31
25-
9
55 0
35
1-73
S-
88
23
5
59-4
Solid
Aatnlunite
M
AMiakAiiite + Na^SO^
<»
•1
M
Aatnkanlte+MfSO^
Solubility of Mixtures of Sodium Sulfate, Potassium Chloridb,
Potassium Sulfate, etc., in Water.
(Meyerhoffer and Saunden, 1899.)
t*.
*4.4
0.2
— 0.4
16.3
24.8
♦16.3
24. 5
03
25.0
♦17.9
♦30- 1
— 21.4
-23.7
— 10.9
— 3
— 3
-14
~I4
-23-3
Sp. Gr. of
Solutions.
Mols. per xooo Mols. HsO.
X.2484
• • •
1.2625
• • •
1.2034
1.2474
1.2890
SO«
5-42
3-35
3-59
4.72
4.37
16.29
14-45
2.75
2.94
13- 84
50-41
1-45
16.25
16.24
1-39
1-39
0.41
Ka Na« Os
14.39 51.83 60.8
12.78 50.93 60.36
16.38 40.75
17-58 50.56
20.00 48.36
9.16 61.06 53.93
9.90 58.46 53.91
25- 77 1793
36.20 14.80
0.0 62.57
10.08 40.33
53-54
63 -42
64.01
40.95
48.06
48.70
0.0
Solid Phase.
KsNa(S04)a+NaaSO«.ioHsO+
KCI+NaCi
NasS04.ioHsO+KCl+NaCl
NasS04.zoHsO+Ka+K«Na(S04)t
K*Na(S04)rfKa+Naa
K:«Na(S04)rl-KCl+NaCI
K«Na(S04)s+NaCl+NasS04.zoHaO+
Na2S04
KsNa(S04)rl-Naa+NajS0t
KsNa(S04)2+KCl+K2S04
K«Na(S04)rhKCl+KaS04
Na9S04.zoHsO+NaaSO«+NaCl
KaNa(S04)rfNaaS04.zoHsO+NaaSQi
46.61 46.36 Naa.sHsO+Na9SO«.ioHiO
10.51 39.58 50.09 NaCl.aHsO+Ka
30.68 ... 29.23 KCl+KaS04
10.03 6.21 ... K«Na(S04)rl-NasS04.zoHsO
10.03 6-21 ... K,Na(S04)rhKsS04
25 -59 8.78 32.94 K,Na(S04)rhNaaS04.ioHaO+Ka
25 -59 8- 78 32.94 KiNa(S04)2+K,S04+Ka
15.15 44.20 58.97 NasSO«.ioHsO+Ka+Naa.aH^
* Indicates tzansition points.
669
SODIUM SULFATE
Solubility of Sodium Sulfate in Aqueous Solutions of Sodium
Acetate at 25®.
(For, 1909.)
Gms. per xoo Gms. Sftt.SoI.
CHiCOONa.
0
Na,S04.
21.9
4.1a
7.71
17.72
16.48
Solid Phue.
NaiSO«.xoH^
11
M
Gms. per 100 Gms. Sat. Sol.
CH,COONa. NaJsoT
12.58 1350
16.26 11.50
20.68 8«io
Solid Phase.
NatSO«.xoHriO
41
U
Solubilitt of Sodium Sulfate in Aqueous Sodium Chloride at 15^
((SchreinemalLerB and de Baat, 1909.)
Gms. per xoo Gms. Sat. Sol.
NaCL
N..SO,.
S-42
7.86
1151
5-87
15-97
S-23
Solid Phase.
NaiSO^xoH^
«
u
Gms. per loo Gms. Sat. Sol.
NaCl.
Na,S04.'
ooua roaae.
21.03
526
NatS04.xoH^
23 -39
5-64
" +Naa
25.21
2.26
NaCl
Solubility of Sodium Sulfate in Aqueous Solutions of Sodium
Chloride at Different Temperatures.
(Seidell, X902.)
Results at I0^
Results at 21
.5^
Results at 27^
Sp. Gr.
Gms. per xoo Gms.
sp. Gr.
of
Solutions.
Gms. per too Gms.
Sp. Gr.
of
Solutions.
Gms. per xoo Gms.
So.
Sohrtiops. KaQ.
NaaSO«.
NaQ.
Na9S04.
kaQ. Na^Q«.
1. 080
0.0
9.14
1. 164
0.0
21.33
1.228
0.0 31.10
1.083
4.28
6.42
1. 169
9 OS
15-48
1.230
2.66 28.73
I. IOC
9.60
4.76
1. 199
17.48
13-73
1.230
5.29 27.17
1.150
15 65
3-99
1. 214
20.41
13.62
1-235
7.90 26.02
1. 164
21.82
3-97
1.243
26.01
15 05
1-259
16.13 24.83
1. 192
28.13
415
1.244
26.53
14.44
I 253
18.91 21.39
1.207
30.11
4-34
1.244
27.74
13-39
1.249
19.64 20.11
1.217
32.27
4-59
1.244
31 25
10.64
1.245
20.77 19.29
1.223
33 76
4. 75
1.243
1-245
1. 219
1. 212
1. 197
31.80
32.10
33 69
34 08
35 46
10.28
8.43
4.73
2.77
0.00
1.238
32.33 9-53
Results at 30^
Resulte at 33^
Results at 35*.
Sp. Gr.
•of
Gms. per
xoo Gms.
IsO.
NaaSO;.
Sp. Gr.
of
Solutions.
Gms. per 100 Gms.
Sp. Gr.
of
Solutions.
Gms. per too Gms.
Solutions.
KaQ.
l^aQ.
NaaSOt.
KaQ. NasSC)
1. 281
0.0
39 70
1.329
0.0
48.48
1.324
0.0 47-94
1.282
2-45
38 25
I 323
1.22
46.49
1. 314
2.14 43-75
1.284
5.61
36.50
1. 318
1.99
45.16
1.256
13.57 26.26
I .290
7.91
35 96
1-315
2.64
4409
1.238
18.78 19.74
I .276
10.61
31.64
I 309
3-47
42.61
1. 231
31.91 8.28
I .270
12.36
29.87
1.265
12.14
29.32
I -193
35-^3 0.00
1.258
15 65
25.02
1-237
21.87
16.83
1.249
18.44
21.30
1.234
32.84
8.76
1.244
20.66
19.06
1. 217
33-99
4 63
1.236
32.43
9.06
1.208
34-77
2.7s
SODIUM SULFATE
670
Solubility of Sodium Sulfate in Aqueous Solutions of Sodium
Chloride at 35*^.
(CameRMi, Bell uid Bohintnn« 1907*)
^ of O/fo^ ner xoo Gnifl. Hd(
Sit.SoL
I. 2173
I. 2162
X.2150
1.227s
I . 238s
I.2S7I
I . 2476
Data are also given for the system 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 Srhrrlnrr, 29x0.)
NaO.
NmS04.
Sniid Phase.
SaLSoL
Naa
N.,S04.
Solid Phue
2.96
26.60
NatSOiJoH/)
1.2429
26.54
12.64
NaaSQ.
579
24.32
M
I . 2438
31.06
9.98
(1
9.90
21. 41
M
1.2451
32.41
9.93
M
1343
19.62
M
I • 2453
33
9.84
« +Naa
iS-82
19.64
«l
1.2309
33.81
6.66
Naa
19- 13
20.73
- +Na,S04
I. 2162
34- 60
3.38
M
23.22
16.28
Na,S04
1.2002
35.80
0
M
(NaOH),.
NaiSO«. '
Solid Phase.
(NaOH)t.
Na,S0..
Solid Phase.
0.074
1. 41
NaiSO«.xoH^
2.82
0.24
NaiSO.
0.70 .
1.08
11
3.52
0.126
u
1-47
0.90
" +Na,S04
5.83
0.013
M
2.02
0.59
Na,S04
6.62
0
Na0H.H^
Solubility of Sodium Sulfate in Aqueous Solutions of Sulfuric
Acid at 25*.
(D'Ans, 1906; X909C; 1913.)
Mds. per
Mols. per xooo Cms.
Sol.
Solid Phase.
Sat.
Sol.
Solid Phase.
H,S04.
NaiSOf.
' SO..
Na«S0|.
0
I. 541
Na,S04.xoH/)
8.70
0.076
NaH«(S04)t.H^
0.286
1. 671
II
8.86
0.156
" .
0.338
1.742
M
8.93
0.273
II
0.60
1.85
W
8.84
0.527
" (unstoUe)
0.763
2
11
8.70
0.808
11 M
0.884
2.256
+Na,S04
8.62
0.844
II M
0.423
0.77
NaSSO^Mfi
8.61
0.899
II
0.496
0.47
II
. 8.87
0.44s
t" +Na,S044*H,SQi
1.666
2.437
Na,S04+Na«H(S0«),
8.93
0.437
Na,S0..4»H.SQ.
1-576
2.363
" +Na«H(S04),.H,0
9.08
0.394
II
2. 611
2.091
Na«H(S04).+ "
9.36
0.425
" +NaH§A
5.91*
0.409
NaHSO«
9.18
0.567
NaHSA
6.30
0.332
II
9.42
0.728
M
6.64
0.297
« +NaH,(S04),.H,0
9.48
0.76
U
6.90
0.173
NaH|<S04)«.H/>
9.48
0.953
" +?
7.36
0.071
II
985
0.787
?
7.74
0.047
II
9.98
0.908
?
8.12
0.037
M
9-77
1.03
WlftuMft
8.40
0.046
11
10.16
0.797
«
10.78
0.302
• Fkom this point on the fipires in this column are Mols.SOk - H1SO4 + SQ|.
100 cc. sat. solution of NatS04 in absolute HtSOi contain 29.99 gms. NasSO«
and the molecular compound which is formed contains 8 mols. H1SO4 per i mol.
NatSOi and melts at about 40^. (Beisiiis. 19x0.)
Aqueous HtSOi containing 0.51 mol. per liter dissolve 2.238 mols. NatSOi per
liter at 25^; Aq. H2SO4 of 0.779 i^ol' P^r liter dissolves 2.465 mols. NatS04 at the
same temperature. (Hen, x9xx-xs^
671
SODIUM SULFATE
Scx^UBiUTT OF Sodium Sulfate in Aqueous Ethyl Alcohol.
(de Bniyn, 190a)
t*
CoDcentxir
tkmof
Cms. Na|S04
Cms.]
[)er 100 Cms. Solutioii.
SoiKl Phase.
9 ■
AkolK^in
Wt. %.
Aq. Akohol.
'h,o.
CsGUOH.
Na«S04.
'.?
0
12.7
88.7
0
II. 3
NaaSO«.xoH^
9.2
6.7
85.1
8.6
6.3
If
€€
19.4
2.6
78.6
18.9
2.5
<i
l<
39-7
0.5
60
39. s
0.5
««
II
5S.9
O.I
41. 1
S8.8
0.1
If
II
72
0
28
72
0
ff
€i
0
37.4
72.8
0
27.2
NatS0«.7H^
II
II. 2
16.3
76. s
95
14
ft
U
20.6
7
74.3
19.2
6.5
fi
II
30.2
2
68.4
29.6
2
If
*.?
0
28.2
78.1
0
21.9
NaiS04.ioH^
II
10.6
13.9
78. s
9.3
12.2
fi
If
24
4.5
72.8
22.9
4-3
ff
II
54
0.4
45-6
54
0.4
" +Na,SO,
36
0
49-3
67
0
33
NaaSO.
If
8.8
29,2
70.6
6.8
22.6
ff
II
12.8
22.4
71.2
10.5
18.3
ff
II
17.9
15.4
71. 1
iS-5
13.4
ff
II
18. 1
^S'S
71
15.7
13.3
f«
II
28.9
5.4
66.5
28.4
5.1
M
II
48.7
0.8
50^9
48.3
0.8
f«
1?
0
47.9
67.6
0
•
32.4
<f
it
9
27.5
71.3
7.1
21.6
l<
U
14.5
19.2
71.8
12. 1
16. 1
ff
II
20.6
12.3
70.6
18.4
10
<f
It
.31
5.1
65.6
29.5
4.9
ff
V
'The following additional determinations
at 25'' are
given by Schreinemakers
and de Baat (1909) :
^?
• • •
• • •
6341
34.84
1.7s
NatS04.xoH/)
If
• • •
• • •
49
SO. 5
0.5
«
II
• • •
• • •
46.6
53
0.4
" +Ni,SQ,
u
• . •
• • •
34.9
64.95
0.15
NdSQi
Between certain concentrations of the aqueous alcohol the liquid separates into
two laye:
rs. The following results were obtained at 25*^
', 36** and 45**:
t".
Upper Layer.
Lower Layer.
Gms.HiO.
, Giiis.CsHcOH.
Gnis.NaaSQ«.
Gins.HaO.
Gms.CsHfiOH. Gms.NaaSO«.
25
66.5
27 -3
6.2
67.4
51
27 S
«
68.1
23 -9
8.0
68.5
6.0
25 S
«
68.3
23.1
8.6
68.3
6.7
25.0
36
• • •
• • •
• • •
66.6
4.1
293
«
57-7
38-4
3-9
• • •
• • •
...
it
65 0
a8.3
6.7
68.8
S-9
35-3
n
68.1
21.2
10.7
68.9
9.4
31.7
45
ti.8
32 -9
5-3
• . •
• • •
. • .
II
65.8
25 -3
8.9
68.4
8.8
22.8
it
66.0
3il.O
10. 0
68.6
10. 1
21.3
Data for equilibrium in the system NatSOi + NaCl + CiHjOH + HiO 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*".
r. 189a.)
Gita,C9RrOB
per zoo Cms.
Akohol-Water
Mixture.
42.20
49-77
55-^5
Gms. Na9S04
ST 100
ms. Sat.
Solution.
1.99
IIS
0.72
Gms. CtBjOR
per 100 Gms.
Alcohol-Water
Mixtuxe.
56.57
60.64
62.81
Gms. NaiSO«
g!r zoo
ms. Sat.
Solution.
0-55
0.44
0.38
100 gms. HtO dissolve 183.7 gms. sugar + 30.5 gms. NatS04 at 3I.25^ or 100
gms. sat. solution contain ^2.2 gms. sugar + 9>6 gms. Na2S04. (Kshler, 2897.)
ICO gms. 95% formic acid dissolve 16.5 gms. NaiS04 at 19^. (Ascfaan, 19x3.)
Solubility of Sodium Sulfate, in an Aqueous Solution of Urea.
(Lfiwienhers, 1895.) .
Solvent.
100 gms. H1O+12 gms. urea
The Conespondinf Fig-
ure for the Solubility
of Na«Sa in Pure Water
Was Found to be:
• • •
21.62
26.48
• • •
32.34
33.09
32.58
Fusion-point data for NatS04 + KCl are given by Sackur (1911-12). Results
for NaiS04 + SrS04 are given by Calcagni (19 12-19 12a). Results for NatS04
+ NajW04 are given by Boeke (1907).
((
tt
it
u
u
ti
u
li
It
u
It
it
f.
20.86
24.83
28.32
29.83
31.90
34.85
39.92
Gms.
NaiSOi per
zoo Gms.
Sat. Sol.
22.36
21.21
26.50
28.23
• ■ •
27 -73
27.19
SODIUM BiSULFATE NaHSOi. (See also last table, p. 670.)
100 gms. HiO dissolve 30 gms. NaHS04 at 16^.
100 gms. HiO dissolve 28.6 gms. NaHSOi at 25° and ^o gms. at lOO*"
100 gms. 95 per cent alcohol dissolve about 1.4 gms. NaHS04at 25^
100 gms. 95% formic acid dissolve 30 gms. NaHSOi at 19.3".
(Aschan, 19x3.)
(U.S. P. VIII.)
, (U.S. P. VIII.)
(Aschan, X9i3*)
SODIUM SULFIDE NatS.9HtO.
Solubility in
Water.
(Pamvano and Fomaini,
1907.)
Gms. NaiS
t*. per 100 Gms.
Sat. Sol.
SoUd Phast.
f.
Gms. Na«S
per 100 Gms.
Sat. Sd.
Solid Phase.
— 10 Eutec
. 9-34
Na«S.9H,0+Ioe
60
29.92
Na,S.s*H.O
+ 10
13-36
Na«S.9H^
70
31-38
(1
15
14-36
<f
80
33-95
II
18
15-30
11
90
37.20
II
22
16.20
u
48
tr.pt
...
NatS.9H^+NatS.6H,0
28
17. 73
u
50
26.7
Na«S.6H^
32
19.09
It
60
28.1
II
37
20.98
u
70
30.22
II
45
24.19
II
80
32.9s
II
48.9tr.pt.
• • ■
« +Na,S.s*Hi0
90
36.42
II
50
28.48
Na,S.5iH,0
91.
5 tr. pt. ...
" +Na,S.s*H^
Fusion-point data for NaiS + S are given by Thomas and Rule (1917).
SODIUM Antimony SULFIDE. See Sodium Sulfoantimonate, p. 627.
673
SODIUM suuin
SODIUM SUIJITE NatSOs.
Solubility
IN
Water.
t
(Haitlqr and Barrett, 1909.)
f.
Giii8.Na|S0k
per xoo Cms.
HdO.
Solid Phase.
f.
Giiis.Na^
per TOO Gms.
H,0.
SoUd Phase.
— 0.76
2. IS
Ice
18.2
2531
Na.S(V7H^
- 1.37
4.21
M
23. 5
29.92
" (mistabk)
— 1.96
6.24
U
29
34.99
fl u
- 2.77
9.44
11
37.2,
44.08
U M
- 35*
12.48
" +Na,SO,.7HdO
21. 6t
...
« +Na.SO^
- 45
17.91
Ice (unstable)
37
28.04
Na,SO,
- 1.9
1309
Na,S0^7H,0
47
28.13
u
+ 2
14.82
••
55.6
28.21
M
59
17.61
'M
59.8
28.76
U
10.6
20.01
If
84
28.26
W
* Eutec.
ttr.pt.
Oxidation was prevented by preparing the material and making the solubility
determinations in an atmosphere ol hydrogen.
Supersolubility curves for the salt are afio given.
The Sp. Gr. of the sat. solution at 15^ b 1.2 1. (Greenish and Smith, x9ozJ
SODIUM HydroSULFITE NatStOi.
Solubility in Water. jeUinck, zgn.)
(vins. N&|S^«
t*. per xoo Gms.
H,0.
SoUd
Phase.
f.
(>ms. N8«S^4
per xoo Gms.
HdO.
Solid Phase.
0. 107 0.
394.
ke
— 4. 58 Eutec.
19
Ice+NaiS^4.3H^
1. 10 4
II
+20
22 (±5% error)
NasSiOi.aH^
2.21 9
II
52 tr. pt.
27.8
" +NS.SJO4
3- IS 13
II
20
24.1
Ns«SiO« (unstable)
4.17 17
II
The pure sample was prepared by salting out the commercial product with
NaCl. It is very easily oxidized to NasSsOs 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 dimculty
was experienced in obtaining concordant results with a given sample of NasSsOi.
SODIUM SULFONATES
Salt.
Solubilitt in Water.
Formula.
Sodiimi:
2.5 Diiodobenzene Sulfonate C6HiIsS0i.Na
Gms.
«e Anhydrous
* ' Salt per xoo
Gms. H|0.
Authority.
3.4
0 Naphthalene Sulfonate
2 Phenathrene Sulfonate
3
10 « "
Phenol Sulfonate
«
* d%^ X.019.
CeHiItSO»Na.HsO
CioHr.SO^a
ti
Ci4H»SO^a.}HsO
Ci4H»SOsNa.HsO
C14Hs.SOsNa.2H1O
CeH4(OH)SO^a.2HsO 15
t ^ » x.o67*
22.5
22.5
239
25
20
20
20
6.82 (Boyle. X909.)
.3.47
6.04 (Fischer, x9o6.)
5.87* (Witt,i9iS.)
0.42 (Sandquist, X9X3.)
I.I "
1.65
14 . 7J (Greenish & Smith/oi.)
19. 2^ (Seidell, xgxo.)
t rf» - X.079
SoLUBiLmr OF Sodium fi Naphthalene Sulfonate in Aqueous Hydro-
chloric Acid at 23. 9^ (Fischer X906.)
Normality of Aq. HO.
X.Ofl.
a«»
3 n.
Sn,
Gms. CioHT.SOsNa perioo gins. Aq.HCl 6.47 5.35 413 2.4a
SODIUM SmiTONATES
674
S(x.UBiLiTY OF Sodium Phenol Sulfonate in Aqueous Alcohol at 2<
(Sddell, 1910)
Gms. CA(0^- Wt. Per cent
SObNall^per CAQHin
100 Gms. Sat SoL Suveai
Sat. SoL
Wt. Per cent
C^dOHin
Solvent.
o(«IU)) 1.079
10 I 054
30 1.030
30 1.004
40 0.977
50 O.Q50
19
17
IS
13
II
9
38
4
5
6
7
7
Iveat.
60
70
80
90
95
100
Sat.SQL
0.919
0.886
0.852
0.820
0.810
0.800
Cms. CtH«(OH>
S0|Na.2H^ MT
zoo Cms. Sat. Sol
75
S-I
2.9
I.I
0.8
.1-5
In the 100 per cent CiHiOH solution, the solid phase, CcHiCOH) S0tNa.2H^,
became opaque.
100 gms. H«0 dissolve 18.25 sn^i* CA(0H)S0tNa.2HK) at 14.8**, ^14.8 of sat.
■ol. - 1.0675.
SODIUM TARTRATES
Salt.
(Gteeniili and Smith, Z9ot0
Solubility in Water.
Fonnula.
20
20
o
Cms. Salt
per zoo Authority.
Gms. H^.
39.73 (Scfakwbeig, 1900.)
41.10 "
0.039 (Fenton, Z89&)
Sodium NeatrallnactivePyrotartrate CiH4(VNat.6HkO
" Dcxtio
Sodium Dihydioxy Tartrate C4H40yNaa.3HsO
SODIUM TELLURATE NatTe04.2HK).
100 ems. HiO dissolve o.f 7 gm. NatTe04 at i8% and 2 gms. at Ioo^ Solid
phase NaiTe04.2HiO.
100 ems. HsO dissolve 1.43 gms. NafTe04 at i8% and 2.5 gms. at 50**. Solid
phase NatTe04.4HiO. (Myli«. z9oz J
SODIUM THIOSULFATE NatSiOi.5HK)(I).
Solubility in Water. (Young and Buke, Z904, Z906.)
Gms. Na^iOfe per
Gms. N14SA per
f>
zoor
Sat. Sol.
^ms. Solid Phase.
Water.
V.
zoo r
'«». Solid Phaaa.
Sat. Sol.
Water.^
0
33.40
5o.i5Na.SA.sH^(D
0
60.47
153 Na«SA.H/)aD
10
37-37
59.66 "
10
61.04
156.7 "
20
41.20
70.07 "
20
62.11
163.9 "
25
i43iS
75-90 "
25
62.73
168.3 "
35
47.71
91.24 "
30
63.56
174.4 "
45
55-33
123.87 "
40
65.22
187.6 «
48.17
*
• • •
. . . "+NaACVaH40(D
50
66.82
201.4 "
0
52.73
III.6oNa.SA.aH/)(I)
56.5*
...
... " +NsAOb
10
53-94
117. 10 "
0
46.14
85 . 67 NaAQi.6Hd0anandIV
20
55-15
122.68 "
10
51.66
106.8 "
25
56.03
127-43 "
13
54.96
122 "
30
57.13
138.84 "
14.35^
1
• • •
... « +NaAQi.lHiO.(IV)
40
59-38
146.20 "
14-3*
• • ■
... « +NaAOb.7HdO<ilJ)
50
62.28
165. II "
0
57-42
I34.8Na«SdQ»7HWnD
60
65.68
191.30 "
10
58.28
139.7 •-
66. s*
• • •
. . . "+ NaAOb
20
59.28
145.6 -
0
41.96
72.30 NaA(VsH/)(II)
25
60.18
151. I "
10
45.25
82.65 "
30
60.78
155 "
20
49.38
97.55 "
40
62.60
167.4 "
25
52.15
108.98 "
47.5^
64.68
183.1"
30
56.57
130.26 "
48.5*
• • •
... f" +NaA0b.HdO(ilJ)
30.22
* ...
... "+NaAO|.4HiO(U)47.5
64.78
183.9 NaiSA.HdCXiiD
33.5
58.59
141.48 NatSA^H^OD
50
65.3
188.2 "
36.2
60.51
153.23 "
55
66.45
198. I "
36.6
62.80 168.82 "
60
68.07
213. I "
40.6s
► ...
,. "+NaAOb.H^(ID 61*
• , .
,,. "+NsAOb
•tr.pt.
675
SODIUM THIOSUIaFATB
Solubility in Water {Continued).
f.
Gffls. Na«£A per
100 Gms.
Sat. Sol. Water/
Solid Phase.
r.
G11M.N1
100
"jSAper
Gms.
. SoKd Phase.
Sat. Sol.
Water.
o
57.63
136
Na,SA.lH^(IV)
30
63.34
172.80
NaAQi.H^(V)
lO
58.49
140.9
It
40
64.75
183.70
«
20
59-57
147.3
(1
50
66.58
199.2
ii
25
60.35
152.2
55^
67.59
208.5
u
30
61.03
156.6
43*
• • •
• • •
«+NaAOb.*H,0(V)
40
62.95
169.9
25
64.21
179.4
NaAQi.»HiO(V)
so
65.45
189. 5
40
64.99
185.6
u
55^
67.07
203.7
SO
66.02
194.3
If
58*
• • •
t • •
" +NaAQi
60
67.4
206.7
<l
0
57.63
136
NaA0b.2HdO(V)
70
69.06
223.2
w
10
59.05
144.2
70*
• • •
• • •
« +NaAOb
20
61.02
156. 5
40
67.4
206.7
Na.SA
as
62.30
165.3
SO
67.76
210.2
u
30
63.56
174.4
60
68.48
217.3
If
35 ^
65.27
188
70
69.05
223.1
f«
27 5^
i
« • •
• • •
" +NaiSA.H^ (V) 80
69.86
231.8
u
•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 grouo 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, NatS|Ot.5HtO (I).
100 gms. alcohol dissolve 0.0025 gm. NaiSsOs and 0.0034 S™* NatSsOi.5HK) at
room temperature. (B{idtker, 2897.)
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 NasSsOt.5HK) by each of the fol-
lowing compounds: urea, glucose, cane sugar, NaCl, NaClOs, NaNOi and NatS04
are given by Bautaric (191 1).
SODIUM TUNOSTATB Na2W04.2HtO.
Solubility
IN Watbr.
(Funk, 1900a.)
Gms.
^0 NatW04 per
• • 100 Gms.
SoludoQ.
Mols.
NatWOi
per
100 Mds.
HsO.
•
Solid
Phase.
Gms.
♦ 0 Na,W04|)er
zoo Gms.
Solution.
-5 30. 60
2.70
NatWO4.xoH40
-3-5 41.67
-4 31 87
2.86
f«
+O.S 41.73
-3-5 32.98
3 01
•i
x8 42 .0
-a 34.52
3 23
a
21 42.27
0 36.54
3 52
t«
43-5 4398
+ 3 39 20
3 95
M
80.5 47-65
5 41 02
426
14
100 49-31
Solid
Phase.
NatW04.aH^
Mols.
NatWOi
zooMols.
HaO.
4.37
4-39
4-40
4.48
4.81
S-57
5-95
Sp. Gr. of sat. solution at 18]* » 1.573. For Sp. Gr. determinations of aqueous
solutions at 20°, see Pawlewski, 1900.
Fusion-point data for NaiWOi + WOt are given by Parravano (1909).
SODIUM URATE 676 »
SODIUM URATE QH|NiOt.Na.
Solubility in Aqueous Sodium Chloridb at 37^
(d'Agostino, 1910.)
Cms. Mols. per Liter.
Cms. Mob
. per Liter.
Gms. Mob. per Liter.
NaQ. CAN40|.Na.
NaCl.
CiH,NANa.
NaQ.
CiH^40t.Na.
0 0.00536
0.01084
0.002II
O.05116
0.00050
0.00486 0.00340
0.01398
0.00172
0.06667
0.00034
0.00533 0.00321
0.02564
0.00102
0.07363
0.00032
0.00865 0.00256
0.04012
0.00054
0.08595
0.00026
M
One liter of HiO dissolves 1.5 gms. sodium urate at 37^. (Becfaholdandiaegier, 19x0.)
One liter of serum dissolves 0.025 gm. sodium urate at 37^ **
SODIUM MetaVANADATE NaVO«.
Solubility in Water.
(MacAdam and Pierle, 191a.)
f.
"^•(Ss:^' Solid Ph.«.
f.
^g'Ss^^ SoUd Phase.
25
21.10 NaVOb
25
15-3 NaVO^aBW
40
26.23 "
40
30.2
60
32.97
60
68.4
75
38.83
75
38.8 NaVOk
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 FluoZIBCONATE 5NaF.ZrF4.
100 gms. HtO dissolve 0.387 gm. at 18°, and 1.67 gms. at 100^. (Mazignac, x86i.)
SPABTEINS CiiHkNs.
Solubility in Water and in Aqx^ous Sodium Carbonate Solutions.
(Valeur, 19x7.)
The author prepared solutions of recently distilled colorless sparteine (a <*
—2^.46' in 5 cm. tube) in aqueous 5 per cent NasCOt and determined the tem-
perature at which clouding occurred in each.
fof
Gms. CuH«Ns
t-of
Gms. Ci»HmNi
fof
Gms. CuHaNf
Qouding.
per 100 cc.
Qouding.
per xoocc.
Qouding.
per 100 oc.
234
2.1
33.5
1.5
47
0.9
24
1-95
36.5
1.35
53
0.7s
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 centrifugation, the amount of sparteine 4n the saturated solution was
determined with the aid of the data in the above table. Enough NasCOs and
H2O to yield 5 per cent NajCOs 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 C»H«N,.HsS04.5HtO.
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 CH,(CH,)i«COOH.
100 gms. HiO 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 -f i% lecithin dissolve 0.2 gm. stearic acid.
In the same solvents there is dissolved of sodium stearate, 0.1, 0.2- and 0.7 gm.
respectively. (Mooxe. Wilson and Hutchinson, Z909O
677 STEARIC ACID
S(H.UBILITT OF STBAKIC AcID IN AqXTEOUS EtHYL AlCOHOL AT 25^^.
(Seidell, 19x0.)
Wt.% j^f Cms. QtHmCOOH Wt. % j ^* Gms. CnHaCCX)!!
CJBW)H cfrSi pcriooGma. OILOH c-Tcii per looGms.
iaSoRent. Sat. Sd. *Sat.SoL iaSofvent. Sat. Sol. *Sat.Sol.
o 0.999 0.034 70 0.865 0.80
20 0.967 0.04 80 0.841 1.63
40 0.932 o.io 90 0.818 3.30
50 O.9II 0.18 95 0.807 5.55
60 0.888 0.40 100 0.795 8.30
loocc. f 94.3 Vol. %CiHjOHcontaino.0996gm.Ci7H»COOHato**(di=o.83i8).
sat. 80I. 95.1 " " " 0.1139 " " " (^,=0.8287).
in 1 95.7 " " " 0.1246 " " " (da =0.8265).
Saturation was approached from above without constant agitation. (Emenon, 1907 .)
SoLUBiLmr OF Stbakic Acm in Ethyl Alcohol at Several Temperatures.
(Faldola, 19x0.)
f.
Gms. CnHMCOOH per 100 cc.
of:
Absolute Alcohol.
75% Alcohol.
50% Alcohol.
10
0.9
0.15
• • •
20
2
• • •
0.08 (23*^)
30
45
0-39
O.IO
40
13.8
0.77
0.12
100 cc. sat. solution in 94.4 Vol. % CHjOH ("methylated alcohol" of (£ =
0.8183) contain 0.15 gm. Ci7Hi8CCX)H at -f 0.2°. Saturation was approached
from above without constant agitation. (Hehner and Mitchell, 1897.)
Solubility of Stearic Acid in Several Solvents at 25*.
(Seidell, 19x0.)
Solvent.
d of Solvent.
c^? c^i PC 100 Gms.
Sat. Sol. »~sat. Sol.
Acetone
<^i»= 0.797
0.815 4.73
Amyl Alcohol (iso)
(feo=o.8i7
0.815 9-43
Amyl Acetate
^0=0.875
0.867 II. 19
Carbon Disulfide
^8= 1.259
I. 163 19.20
Carbon Tetrachloride
<i28= 1.587
1.465 10.25
Chloroform
dn= 1.476
I 332 15- 54
Ether (abs.)
4a=o.7ii
0.744 20.04
Ethyl Acetate
<^= 0.892
0.895 7.36
Nitrobenzene
dn= 1.20s
1 . 199 1 . 24
Toluene
Ji6= 0.872
0.865 13 61
Fusion-point data for stearic
: acid + tristearin and for stearic acid + tri-
stearin + palmitic acid are given by Kremann and Kropsch (1914).
STILBENE C6HftCH:CH.C6Ht.
Freezing-point data for mixtures of stilbene and p dimethoxystilbene are given
by Pascal and Normand (19 13).
STBONTTOM ACETATE Sr(CH,CCX)),.}H,0.
Solubility in Water.
(Osaka and Abe, 19 11.)
*•• 1S'i«SS?S' Solid Ph«e. f. ^i4'<^5C^« SoBdPta«.
0.05 36.93
Sr(CH«C00)i4H«0
25
40.19
Sr(CH|COO)t.iH/>
S 39- 91
«
35.03
38.82
11
10 43 . 61
II
50
37. 35
II
8.4 tr.pt. 43. 1
" +Sr(CH,COO),.|H,0
70
36.24
M
8 43.5
Sr(CH|COO)i.iH,0
80
36.10
«l
10 42.95
u
90
36.24
a
15 41.90
II
97
36.36
«
STROMTZUM BENZOATE 678
STBONnUM BENZOATE Sr(C7HtOt)2.HK).
SoLUBiLmr IN Water.
(Pajetta, 1906.)
*•■ 15.7*. 24-7*. 314*. 40-9*.
Gms. Sr(C7H80s)s per 100 Gzns. Solution $-3^ S-4 S-S^ 5*77
STBOMTIUM BBOMATE Sr(BK)i)t.
One liter of aqueous solution contains 0.9 gm. molecules or 309 gms. Sr(BrOs)i
at I8^ (KohlnHMch. z897-)
STBONTIUM BBOMIDE SrBrt.6HK).
Solubility in Water.
(Avenge curve from results of Kremecs, 1858; and Etaid, 1894.)
Gms. SrBri per 100 Gms. Gms. SrBri per loo Gms.
» .
^ution.
Water.
0
46
85.2
10
48.3
93
20
SO. 6
102.4
25
51-7
107
30
52.8
III. 9
• .
Solution.
Water.
40
SO
60
80
SS'2
S7.6
60
64- s
123.2
13s. «
ISO
181. 8
100
69
222. S
Sp. Gr. of sat. solution at 20° approximately 1.70.
100 gms. abs. alcohol dissolve 64.5 gms. SrBri at o^. Sp. Gr. of solution » i .21.
(Fonaes-Diaoon, 1895.)
Solubility of Strontium Bromide in Aqueous Solutions of Strontium
Nitrate at 25°.
(Harkins and Pearce, 1916.)
Mols. per zooo Gms. H|0. Gms. SriBr, j ©f Mols. per 1000 Gms. H|0. Gms-SrSr, j o|
' „ ,...^ V * r, -^ ^ per 1000 Gms. _ Tr_ . < _ .---. " „ ^ » per xooo Gms. « Tr« ,
Sr(NOj),. SrBr,.: _ HA Sat. SoL Sr(NQ,)|. SrBr,. "^ h^. Sat. Sol.
o 4.3080 1066. I 1.7002 0.30663 4.3180 1068.8 1.73766
0.036 4-3105 1066.95 ... O.61124 4.3190 1069.17 1.74866
0.07216 43125 1067.42 1.70325 1.8610 43390 1073.97 1-77368
0.14568 4.3170 1068.54 1.72844
Data for equilibrium in the system strontium bromide, strontium oxide and
water at 25" are given by Milikau (19 16).
STRONTIUM CAMPHORATE d CioHi404Sr.4HtO.
Solubility in Aqueous Solutions of Camphoric Acid at 16-17*.
(JuDgflcisch and Landrieu, 1914.)
Gms. per zoo Gms. Sat. Sol. „ ,. . ». Gms. per 100 Gms. Sat. Sol. „ .. . «.
, *• % Sobd Phase. e * ■ » Solid Phase.
(CHmCCOOH),. CioHM04Sr. CsHm(COOH),. Q^ElMQiSr. ^"" -^""w-
1.25 1. 413 C.Hm(COOH), 1.20 17.99 (C»H,/)4),SKCiiH,^J,
1.03 1.7705 (CioHu04)»Sr(C»Htf04)s O 16.95 QoHuOfSr^B^O
1. 13 6.525 " o 16.56
1.20 12.452 O 12.86 (at98*) "
STBOMnUM CARBONATE SrCO,.
One liter of water dissolves 0.00082 gm. at 8.8** and 0.0109 gm. at 24* by con-
ductivity method. (Holleman, 1893; Kohkausch and Rose, 1893.)
One liter of water saturated with COi dissolves 1.19 gms. Sr(HCOi)i.
Data for the solubility of strontium carbonate in water containing COi at
pressures between 0.05 and i.i atmospheres are given by McCoy and Smith
(1911). The equilibrium constant is ife = 1.29 X lo"* 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 COi = *a = 1.567 X lO"*.
679
STRONTIUM CARBONATE
Solubility of Strontium Carbonate in Aqueous Ammonium Chloride.
(Cantoni and Goguelia, 1905.)
Cms. NH«a ^
100 Gms. Solutioo.
Gms. SrCX)i per
1000 cc. Sat. Solutioii.
S'3S 0.179
10 0.259
20 0.358
The mixtures were allowed to stand at 12-18^ for 98 days.
Fusion-point data for SrCOi + SrCli are given by Sackur (1911-12).
STRONTIUM CHLORATE SrCClO.),.
100 gms. HiO dissolve I7d..9 gms. Sr(C10)t, or 100 gms. sat. solution contain
63.6 gms. at 18". Sp. Gr. of solution is 1.839. (Mylius and Funk, 1897.)
STRONTIUM CHLORIDE SrCls.6H,0.
SoLUBiLmr IN Water.
(Average curve from the results of Mulder; Etard; see also TOden, 1884.)
t*.
Gms. SrQ]
1 per 100 Gm
•• Solid
"* Phase.
t*.
Gins.SrCl]
1 per 100 Gms.
Solid
'Solutkn.
Water.
'Solution.
Water.
Phase.
— 20
26.0
351
SrCls^6H«0
60
45 0
81.8
Sras.6HsO
0
30.3
43 S
m
70
46.2
85 -9
Srds^H^O
10
32 -3
47-7
M
80
47-5
905
M
20
34-6
52 -9
w
100
50.2
100.8
••
25
35-8
55-8
M
120
53 -o
112. 8
M
30
37 0
58.7
U
140
55-6
125.2
«
40
39 S
65 -3
M
160
585
141 .0
m
50
42.0
72.4
M
180
62.0
163. 1
m
Transition temperature about 62.5^ Sp. Gr. of sat. solution at o^ <- 1.334; &t
15* =• 1.36.
Solubility of Strontium Chloride in
Hydrochloric Acid at o**.
Mg. Mols. per yo cc. Solutiop.
iSrOs-
51.6
44.8
37 85
27.2
22.0
14.0
425
HQ.
O
6
12
23
28
37
52
I
75
3
38
25
75
Sp. Gr. of
Solutioo.
I
I
I
I
I
I
I
334
304
269
220
201
167
133
Aqueous Solutions op
(Engel, z888.)
Grams per xoo cc. Solution.
SrOa.
HQ. '
40.9
0.0
35-5
2.22
30. 0
4-65
21.56
8.49
17.44
10 -35
11.09
J3-58
3-37
19 23
Solubility of Strontium Chloride in Aqueous Solutions op
bromic and of hydrochloric acids at 25*^.
(Harkins and Paine, 19x6.)
Hydro-
In Aqueous HBr.
Gms. Equiv. HBr
per xooo Gms.
O
rf„of
Sat. Sol.
0.06817
O.419I
0.9716
1. 154
1.40x5
1.4020
1 .4010
1.3992
1-3995
Gms. SrCls
per xoo Gms.
Sat. Sol.
3580
35.47
33-9^
31.52
20.78
In Aqueous HCl.
Gms. Equiv. HCl j,, of
per xooo Gms.
HtO.
O.1551
0.5162
1. 017
2.165
9.205
Sat. Sol.
1-3953
1.3788
1.3563
1.3065
I . 1498
Gm8.SrCli
per 100 Gms.
Sat. Sol.
35.17
33.60
31.42
26.33
3.055
STRONTIUM CHLOBmE
680
Solubility of Strontium Chloride in Aqueous Solutions of Acids
AND OF Salts at 25^.
(Haikins and Paine, 19 16.)
Aqueous
Solution ,
of: 1
Gms. Equhr.
addedSalt
[)er 1000 Gms.
Sat. Sol.
Gms. SrCIt
per xoo Gms.
Sat. Sol.
Aqueous
Solution
of:
Gms. Equiv.
added Salt
per 1000 Gms. <
Hfi,
rf of Gms-SrO.
'Tc 1 periooGms.
>at. Sol. »sat. Sol.
CuClt
0.7134 ]
[.4200
34.005
KNQg
0.09796 I
.4107
35-86
n
2.276 ]
^•4595
30.40
tt
0.4755 I
.4349
3590
HT
O.164I ]
[ .4058
34.850
HNQ,
O.I771 I
.4038
3552
(I
0.4462 :
[.4121
33-28
tt
0.3521 I
.4059
35 40
it
0-7S39 ^
[.4196
31-52
tt
1.277 I
.4175
34 04
KT
0.09199 ]
C.4093
35-45
NaNO,
0.3621 I
.4216
35 63
ii
0 . 5401 ]
[.4466
33-79
<<
0.5010 I
.4588
35-60
It
0.6015 3
^•4513
33 -60
tt
3.553 I
.5214
30.88
U
1.445 3
^•5154
30.90
tt
6.856 I
.5581
25 -53
KCl
0.0719 ]
C.4032
35.62
Sf(NO,),
0.1372 I
.4113
35-42
tt
0.433 3
C.4085
34.80
((
0.5766 I
•4336
34.47
it
0.8576 ]
[.4152
33 89
tt
1.0988 I
.4636
33-30
tt
1-594 1
[.4266
32.40
tt
3.318 I
.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. SrCls.6HsO at 6**.
100 gms. abs. ethyl alcohol dissolve 3.8 gms. SrCls.6HsO at 6^. (de Bruyn, xSga.)
Solubilitt of Strontium Chloride in Aqueous Ethtl Alcohol
Solutions at iS**.
(Gemxdin, 1865.)
Sp. Gr. of
Lq. Alcohol
ate*.
Wt.
per cent
Alcohol.
Gms. SrGt
per TOO Gms.
Alcohol.
Sp. Gr. of
Aq. Alcohol
ato*».
Wt.
percent
Alcohol.
Gms. SrOs
per zoo Gms.
AlcchdL,
0.990
6
49.81
0.939
45
26.8
0.985
10
47-0
0.909
59
19.2
0.973
23
39-6
0.846
86
4.9
0.966
30
35-9
0.832
91
3-2
0.953
38
30.4
ns. 95% formic acid dissolve 23.8
gms. SrCU at
19".
100 cc. anhydrous hydrazine dissolve 8 gms. SrCls at room temp.
(Welsh and Brodeiaon, 1915.)
Fusion-point data for SrCl« + SrFj are given by Plato (1907). Results for
SrCl, + SrO and SrClj + SrSOi by Sackur (1911-12). Results for SrCl, + TlCl
by Korreng (1914) and results for SrCU + ZnCls by Sandonnini (1912a, 1914).
STRONTIUM CHBOMATE SrCr04.
Solubility in Water, etc., at 15**.
(Fresenius, 1891.)
Gms. SrCr04
Solvent.
per 100
Gms. Solvent.
Water
0.12
Aq.NH4Cl(s%)
0.19s
Aq. CHsCOOH (1%) 1.57
Gms. SrCiOi
S(4vent. pwr zoo
Gms. Solvent.
Aq. Ethyl Alcohol (29%) 0.0132
Aq. Ethyl Alcohol (53%) 0.002
68i STBONTIXTM CINNAMATE
STRONTIUM CINNAMATE (C6H6CH:CH.COO)jSr.2H,0.
100 gms. H,0 dissolve i gm. (C«H.CH:CH.C(X))jSr at i5*'-20**.
(Squire and Caines, 1905.)
100 gms. sat. aqueous solution contain 1.18 gm. (CeHtCH:CH.CC)0)tSr at 15
and 3.1 1 gms. at 100®. (Tanigi and Checchi, 1901.)
STRONTIUM FORMATE Sr(HC00),.2H,0.
Solubility in Water. (Stanley, 1904)
O 7.02 (8.3s) Sr(HC(X))t.2H^ 67.5 20.62 (21.76) Sr(HC(X))t.2H|0
II 8.08(9.54) " 81. 5 26.14(26.36)
28.6 11.62(13.25) " 86 27.58(27.57) Sr(HCCX)),.HjO
37.4 13.01(14.68) " 91.7. 27,01(27.07)
51.4 16.31(17.83) " 100 26.57(26.72)
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 SrS04 recorded in the original table and
show the weight of Sr(HCOO)s per 100 gms. of saturated solution.
STRONTIUM FLUORIDB SrF,.
One liter of water dissolves 0.1135 gm. SrFt at 0.26°, 0.1173 8^™- at 17.4** and
0*1193 S™* at 27.4°, determined by the conductivity method. (Kohlrauach, 1908.)
STRONTIUM QLYCEROPHOSPHATE C,H70,P04Sr.2H,0.
100 gms. sat. solution in water contain 2.09 gms. anhydrous salt at 18** and 0.8
gm. at 60°. (Rogier and Fiore, z9x.i.)
STRONTIUM HYDROXIDE Sr(OH)t.8H20.
Solubility in Water. (Scfadbier, 1883.)
^ Grams per lOo Grams Solution. Grams per loo cc. Solution.
SrO^ Sr(OH)a.8HaO.'
o 0.35 O
10 048 I
20 0.68 I
30 I .00 2
40 I .48 3
SO 2.13 5
60 3 .03 7
70 4-35 II
80 6.56 16
90 12.0 30
100 18.6 47
90
23
74
57
80
46
77
16
83
78
71
' SrO.
Sr(OH)2.RHaO.
0.35
0.90
0.48
1.23
0.68
1.74
1. 01
2-59
I-5I
3 87
2.18
5 59
3.12
8.00
455
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. HjO. . Gms. per xoo Gms. H|0.
Sa?*&l SrOas ' rfNO,^ ^^ ^*^' sJ*^ SrOas
5>at. S)Ol. Sr(0H),. =>'^^W«- Sat. Sol. Sr(0H),.
1. 481 O 79.27 Sr(NOi)s 1-267. I. II
1.492 0.38 79.47 " 1. 217 1. 01
1.494 0.78 80.83 " 1. 178 0.95
1.506 1.76 81.06 Sr(0H)t.8H|0 1. 148 0.91
1.490 1. 71 74-27 " 1. 108 0.84
1. 419 1.51 63.71 " 1.079 0.81
1.381 1. 41 56.30 " 1059 0.79
1.327 1.27 46.97 " 1.033 0.78
SoUd Phase.
Sr(NOi)s.
37.81
Sr(OH)t.8HiO
28.80
<i
23.83
II
17.96
II
12.78
II
8.96
M
6.29
II
4.45
M
STKONXiUM BTDBOZIDE
683
Solubility op Strontium Hydroxide in Aqueous Solutions at 25*
(Rnthmund, 191a)
Mob.
Gmt.
Mob.
Cms.
AqoMin SdutioB of:
"9-
Sr(OH),
Aqueous Sofaitioo of :
"^
Sc(OH),
per Liter.
liter.
per Liter.
Lhtf.
Water alone
00835
10.16
0.5 n Glycol
0.0922
II. 21
0.5 n Methyl Alcohol
0.0820
9.97
" Glycerol
0.1094
13.31
" Ethyl Alcohol
0.0744
9.05
'' Mannitol
0.1996
24.29
" Propyl Alcohol
0.0708
8.61
" Urea
0.0820
9.97
" Amyl Alcohol
" Ammonia
0.0785
9. 55
(tertiary)
0.0630
7.66
*' Dimethylamine
0.0586
7.13
" Acetone
0.0693
8.42
" Pyridine
0.0694
8.44
" Ether
0.0645
7.85
Data for equilibrium in the system strontium hydroxide, phenol and water at
25* are given by van Meurs (19 16).
lODATI Sr(IO«),.
100 gms. HsO dissolve 0.026 gm. at 15^, and 0.72-0.91 gm. at loo^
((kiy-Lusaac; Rammrlnheri, 1858.)
8TBONTIUM lODmE SrI,.6H,0.
Solubility in Water.
(Avenge curve from the results of Kfemeis, 1858; and Etard, 1874.)
*• Mm.
Gms. Sris per 100 Gms
Solid
■* Phase.
t«.
Gms. Srli per
xoo Gm«.
Solid
• . ^
Solutiaa. Water.
Solution.
Water.
Phase.
0
62.3 165.3
SrItj6HaO
90
78 s
365-2
SrIs.sH^
20
640 177 -8
M
100
79-3
383-1
M
40
65 -7 191-5
M
120
80.7
418. 1
M
60
68.5 217.5
M
140
82.5
471 -5
M
80
73.0 270.4
U
175
85.6
594-4
m
Transition temperature about 90^. ^ Sp. Gr. of sat. solution at 20^ » 2.15
100 gms. sat. solution of strontium ioaide in absolute alcohol contain 2.6 gms.
Srif at —20*, 3.1 ems. 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 PerlODmE Srl«.
Data for the formation of strontium periodide in aqueous solution at 25^
are given by Herz and Bulla (191 1). The experiments were made by adding
iodine to aqueous solutions of Sris and agitating with carbon tetrachloride.
From the iodine content of the CCI4 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 lODOMERCURATI SrIt.HgI..8H,0.
A saturated aqueous solution prepared by adding Srlt and Hgis in excess to
warm water and filtering when the temperature had fallen to 16.5** was found
to have the composition 1.0 Srls.1.24 Hgls.18.09 HsO. The du,g was 2.5
(Dttboin, Z906.)
683
STRONTIXTM BfiALATE
STRONTIUM BfiALATE SrC«H40B.
Solubility in Water.
(Cantoni and Basadonna, 1906.)
f.
Gms. per zoo
t^
Cms. per 100
cc. Solution.
ft®
Gms. per xoo
cc. Solution.
V •
* .
cc. Solution.
20
0.448
40
1-385
55
2.460
25
0-550
45
1-743
60
2.821
30
0.752
SO
2.098
65
3 -143
35
1.036
70
3-360
ON-
nui
I BAALONATI CH,(COO)tSr.
Solubility in Water.
•
(Cantoni and Diotalevi, 1905.)
«•
Gms. per xoo oc
*•
Gms. per xoo cc.
r.
Gms. per 100 cc.
v .
Sat. Sol.
• .
Sat. Sol.
Sat. Sol.
0
0.541
25
0.521
40
0.464
10
0.540
30
0.499
45
0.453
20
0.532
35
•
0.478
50
0.443
STRONTIUM MOLTBDATI SrMoOi.
100 gms. H2O dissolve 0.0104 gm. SrMoOi at 17^
STRONTIUM NITRATE Sr(NO«)i.
Solubility in Water.
(Bericeley and Appleby, 19x1.)
Gms.
Sr(NOi)iPer
100 Gms. H^.
40.124 Sr(N0^s.4H^
60.867
(Smith and Btadboiy, 1891.)
r.
0.58
14.71
26.40
29.06
29 -3*
30.28
32.58
dtOt
Sat. Sol.
I . 28561
I . 39380
I. 4883 I
I. 51098
■ • •
I.51441
1. 51408
Solid
Phase.
r.
dtOi
Solid
82.052
87 . 648
88^577
88.943
K
«
<l
+Sr(NO,),
Sr(NOi)i
3074
47-73
61.34
68.96
78.98
88.94
1. 51282 90.086 Sr(N0i>t
I.51150 91.446
I. 51048 93.856
I. 51057 95- 576
I.51091 97.865
I.51174 100.136
((
II
II
II
(I
The determinations were made with very great accuracy.
Solubility of Strontium Nitrate in Aqueous Alcohol at 25^
(D'Ans and Siegler, X913.)
Wt.% Gms. per 100 Gms.
CJLOHin Sat. Sol.
SoUd Phase.
Wt.%
qaoHiii
Solvent.
(jms. oer 100 Gms.
i Sat..Sol. Solid Phase.
Sdvent.
CiHiOH. Sr(NOa)t.
CHfOH.
SrCNOOi.
0
0 44-25 Sr(NO|>,waiiO
10
6
40.05 Sr(NOk), (unstable)
4
1.7 42.8
II
18.8*
9.5
36.7 " (unsUble)
6
2.6 42.1
II
12.35
34-3 " +Sr(N0j),.4H«0
10.8
4-95 40.4
II
20.6
13.8
33 • 2 Sr(NO,),
16
7.95 37.6
II
40.65
32.35
20.5
20*
12.35 34.3
" +Sr(NCW«
59.9
53.6
10.5
0
0 46.6
Sr(NOi),(unsUble)
79.2
77.15
2.6 "
6
3-45 42.7
II II
99.4
99.38
0.02 "
• Tr. pt,
too CC. anhydrous hydrazine dissolve 5 gms. Sr(NOi)t at room temp.
(Welsh and Broderson, 19x5.)
STRONTIUM NITRITE Sr(NO0s.HsO.
100 cc. sat. solution in water contain 62.83 i^s. Sr(NOi)t.H|0 at 19.5^
" 90% alcohol " 0.42 " " " 2o<
" abs. alcohol " 0.04 " " " 20^
(Vogel, 1903.)
<«
tt
II
STRONTIUM NITRITE
684
Solubility of Strontium Nitrite in Watbr.
(OtwaM, Z9X2,
1914.)
Cms. Sr(NOi),
Gms. SrCNO,),
r.
per zoo Gnu.
Sat. Sol.
Solid Phase.
r.
per looGmii
Sat.SoL
Solid Phase.
- 1.3
II. 3
Ice
35
43.1
Sr(NOk)|.H/)
- 31
19
6
M
52. 5
46.5
(1
- 7.7
35
5
«
60.5
49-3
M
- 6.8
32
8
" +Sr(NO^,.H/)
65.5
SO. 7
W
- 2.3
33
4
Sr(NCMt.H/)
82.5
54
M
- 0.3
34
5^
<f
92
56.6
M
+19
39
3*
II
98
58.1
M
* tf i- Z.446X.
STRONTIUM OXALATE SrC,04.HsO.
One liter of water dissolves 0.0328 em. SrCf04 at 1.35% 0.0^^ gm. at 15.0%
0.0461 gm. at I8^ 0.0575 gm. at 31.7^ and 0.0617 gm. at 37.3^ determined by
the conductivity method. (Kohlrausch, 1908.)
One liter of sat. aqueous solution contains 0.057 gm. SrCs04 at o^ 0.077 gm.
at 20® and 0.093 gm. at 40^ (Cantoni and Diotalevi, 1905.)
Solubility of Strontium Oxalate in Aqueous Acetic Acm Solutions
at 26*-27*.
(Hexz and Muha, 1903.)
Normality oi
Acetic Aad.
O
0.58
1-45
2.89
Cms. per xoo cc. Solution.
CHiCOOH.
O
3.48
8.70
17 -34
SrQO«.H«0.
0.009
0.0526
0.0622
0.0642
Normality ot
Acetic Aad.
3.86
5.79
16.26
Gms. per zoo cc. Solution.
CH,C0OH.
23.16
34.74
97.56
SrCA.HA
0.0598
0.0496
0.0060
STRONTIUM OXIDE SrO.
Fused SrCU dissolves 18.3 gms. SrO per 100 gms. of the fused melt at 910^
(Amdt., 1907.)
STRONTIUM PERMANGANATE Sr(Mn04)s.
100 gms. of the sat. solution in water contain about 2.5 gms. Sr(Mn04)i at o^
(Patterson, Z906J
STRONTIUM SALICYLATE (C«H40H.COO)tSr.2HsO.
100 gms. sat. solution in water contain 3.04 gms. (C6H40HCOO)tSr at 15* and
20.44 gms. at 100^ (Tamgi and Checchi, Z90Z.)
Solubility of Strontium Salicylate in Aqueous Alcohol at 25*.
(Seidell, z^9, 19x0.)
Wt. %
CJLOHin
Solvent.
Sat.S(d
Gms. (C:9H«.0H,
C(X))?r.aHiO
per zoo Gms.
Sat. Sol.
0
10
1.022
1.006
504
4.88
20
30
40
50
0.993
0.982
0.966
0.948
5.22
6.20
7.70
8.08
Wt. %
qiLOHin
Solvent.
dnoi
Gms. (C|HX)H-
C(X))tSr.2H/)
Sat. Sol.
per xoo Gms.
Sat. Sol.
60
0.923
7.15
70
0.893
5.90
80
0.859
4.40
90
0.824
2.56
92.3
0.815
2.02
TOO
0.790
0.44
The solid phase was (C6H40H.COO)sSr.2HsO in all cases except the solution
in 100 per cent alcohol, in which partial dehydration and conversion of the
crystalline salt to an amorphous bulicy white powder occurred.
685 STRONTIUM SUCCINATE
STRONTIUM SUCCINATE CiHtOiSr.
100 gms. sat. solution in water contain 0.439 gm. C4H404Sr at is** and 0.215
gm. at 100**. (Tanigi and Checchi, xgoz.)
Solubility of Strontium Succinate in Water.
(Cantoni and Diotalevi, 1905.)
Gms. C4H«04Sr
t*. per xoo oc
Sat. Sol.
40 0.37s
45 0.389
50 0.424
r.
Gms.C4H^4Sr
per zoocc.
Sat. Sol.
f.
Gms. QHiOtSr
per zoocc.
Sat. Sol.
0
5
0.052
0.076
20
25
0.270
0.382
10
O.III
30
0.451
IS
0,177
35
1 f^ #-«^^
0.413
One liter of water dissolves 0.1133 em. SrS04 at 2.85®, 0.1143 gm. at 17.4*
and o. 1 143 gm. at 32.3**, determined by tne conductivity method. (Kohlzauacli, zgoS.)
Solubility of Strontium Sulfate in Aqueous Solutions of Ammonium
Acetate at 25*.
(Maiden, Z9z6.)
Gma. per zoo Gms. Sat. Sol. Gms. per zoo Gms. Sat. Sol.
CH«C0ONH4. SrSO*. CHtCOONH,. SrSO*.
o 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, Z9Z5.)
Analvzed solutions of Sr(NOi)s» Ca(NOs)s and CaS04 were mixed at 60^ and
allowed to stand at room temperature i to 2 days. The resulting SrSOi was
determined and the difference between the amount found and the amount
which would have resulted if all the Sr(NOs)t had been converted to SrS04,
was taken as the amount of SrS04 dissolved. Gradually increasing concentra-
tions of Ca(NOi)s were used.
Gms. per zoo cc. Sat. Sol. Gms. per zoo cc. Sat. Sol.
'Ca(NOa)s. ' SrSO*. 'Ca(NO,),. ' SrSO*.
0.5 0.0483 4 0.1489
I 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, Z884.)
ec. of Aq. In Aq. HQ In Aq. HNQt In Aq. CHaaCOOH In Aq. HCOOH
Aaa con- Gms. per zoo cc. Gms. per zoo cc. Gms. per zoo cc. Sol. Gms. per zoo oc.
S?^"- Sol. Sol. ' ^H^Q * • Sol.
bSuSaue! HQ. SrSO«. HNOt. SrSoT COOH. ^^*' HCOOH. SrSOi.
0.2 18.23 O.161 31 52 0.381
o-s 7.29 0.207 12.61 0.307
10 3.65 0.188 6.30 0.217 94
2.0 1.82 0.126 3.15 0.138 47
zo.o 0.36 0.048 0.63 0.049
100 gms. 95 per cent formic acid dissolve 0.02 gm. SrS04 at 18.5*. (Aacfaan, 1913)-
47 0.026 46
23 0.022
02 0.024
8TBONTIUM SULFATE 686
SOLUBILITT OF STRONTIUM SULFATE IN AqUBOUS SoDIUM CaSBONATB AT 25^
(Hen, X9ZO.)
Freshly prepared and dried SrS04 was shaken 5 days with aqueous sodium
carbonate solutions and the supernatant clear solutions analyzed.
NonnalHy of Aqueous ^™- ^o^- P^ ^^^^ Sat. Sol.
NhCO* (^h^) . ^ ^^
\ a / a 2
0.6025 0.0382 0.5643
1.305 0.076 1. 139
3.41 0153 2.257
Solubility of Strontium Sulfate in Sulfuric Acid Solutions.
r. Cone of H^,. ^""G^ASd.'^ Authority.
ord. concentrated 5.68 (sturve, 1870-)
" fuming 9.77 "
91 % 0 . 08 (Varemie and Paukan, 1881.)
(t
70 Sp. Gr. 1.843 = 99% 14 (Ganide. 1875.)
ord. Absolute H^04 21.7* (Bergiua. 1910.)
* per zoo oc Sat. SoL
Solubility of Strontium Sulfate in Aqueous Salt Solutions.
(Vizdk, 1863.)
InAq. NaQ. In Aq. KO. InAq. MgOg. InAq. CaCl|.
(a.) (6.) (a.) (6.) (a.) (6.) («.) (6.) '
8.44 0.165 8.33 0.193 1-59 0.199 ^-^7 0.176
15.54 0.219 13.54 0.193 4.03 0.306 16.51 0.185
33.17 0.181 18.08 0.351 13*63 0.243 33- 70 0.171
(a) = Gms. salt per 100 gms. aq. solution, (b) » Gms. SrSOf per 100 gms.
solvent.
STRONTIUM TARTRATE SrCAOe-sHiO.
Solubility in Water.
(Cantoni and Zachoder, 1905.)
Gms. Gms. Gmi.
r. SrCtHA-3H|0 per I*. Sx€«H«0h;3H«0 per t*. SrQEUOL^HfO per
zoo cc. Solution. xoo oc Solution. xoo cc. Solution.
O O.II3 35 0.224 60 0.486
10 0.149 30 0.253 70 0.580
15 0.174 40 0.338 80 . 0.688
30 0.300 50 0.407 85 0.755
Solubility of Strontium Tartrate in Aqueous Solutions of Acetic Acid
AT 36*-27''.
(Hera and Muhs, 1903 •)
Normality of Gms. per loocc Solution. Normality of Gms. per loq cc Solution.
AceticAdd. CHiCOOH. SrC«HA4^- AceticAdd. CHiCOOH. SrG|HA-3H^.
o o 0.337 3.77 21.85 1. 051
0.5^5 3-39 0.678 5 65 33 90 0.983
1.435 8.15 0.864 16.89 101.34 0.184
3.85 17.10 0.996
STRONTIUM (Di) TUNGSTATE SrWA.3HiO.
<
100 cc. HfO dissolve 0.35 gm. at 15^ (Lefort. 1878.)
687
8TBYCHNINS
8TBTCHNINB CuHsN A.
SoLUBiuTY IN Several Solvents.
Solvent.
Water
«
it
Aq. io%NHi
Aq. 3% HjBO» in 50%
Glycerol ord.t.
CtHtOH «=o.83)
" W-0.83)
" W-0.83) 25
+io%NHi 20
GiBs.Cii%NA
t*. per zoo Gms.
Solvent.
«
3-5
15-20 0.71
20 0.833
0.91
0.256
25 0.70
25 0.49
20 20
25 OSS
20 0.77
25 0.76
(z) Baioni and Barlinetto (zQzz); (2) ZaUi
(1993); (6) Schaefer (z9z3); (7) Squue and
Scoindelinaaer (x9oz); (zi) Holty (Z905).
CH^H y =0.796)
Aniline
Amyl Alcohol
Benzene
(t
r
3J
4)
3
61
(3)
(4)
6
Solvent.
Carbon Tetrachloride 20
«
It
Chloroform
(I
Diethylamine
Ethyl Acetate
Ether
(I
" sat. with HiO
Glycerol
Petroleum Ether
Piperidine
P3Tidine
Aq. 50 % Pyridine
Water sat. with Ether
CM! of Sesame
t-.
Gms.Cn%NA
per zoo Gins.
Solvent.
20
0.158 (s)
20
0.22 (9)
17
0.645 (10)
2S
10. 25 16)
25
16.6 (14)
20
1-7 (3)
20
0.197 (s)
20
0.043 (s)
25
0.018 (4)
20
0.051 (5)
IS
0.25
20
0.0093 M
20
0.7 (3)
20
i-S (3)
26
1 . 24 (11)
20-25 2.43 (8J
20
0.017 \s)
20
0.061 (2)
LZQzo); (3) Scholtz (zgzi); (4) U. S. P. 8tli ed.; CO MOller
(190S); (8) Dehn (igz?); (9) Gori (Z9Z3); (zo)
Solubility of Strychninb in Aqueous Alcohol at is'-ao*.
(Squire and Caiiws, Z905.)
Per cent Alcohol in Solvent so 45 60 70 90
Gms. C2iHsNs02 per 100 CO. solvent 0.024 0.125 0.25 0.40 0.59
SOLUBIUTY OF StRYCHNINB IN MIXTURES OF EtHBR AND CHLOROFORM AT 35^
(Maiden and Dover, 1916.)
Percent
CHCUin
Mixed SMvenL
100
90
80
70
60
Gms. G«|IL|NA
per zoo Gms.
Mixed Solvent.
153
7.1
2.77
IS
0.65
Per cent
CHCIain
Mixed Solvent.
SO
30
30
10
o
Gms. Cn%NA
per zoo Gms.
Mixed Solvent.
o.'3S
0.21
o.is
0.09
0.02
SOLXTBILITT OF STRYCHNINE IN MiXED SOLVENTS AT 25"*.
(Schaefer, Z9Z3.)
Mixture.
One volume of CiH60H+4 vols. CHCU
One volume of C»H60H-|-4 vols. CtHe
One volume of CHjOH +4 vols. CHCU
One volume of CHgOH +4 vols. CeHe
Gm. Cii^J<M3b per
zoo oc oiAuxture.
S
2S
6.7
DiSTBIBUTION OF STRYCHNINE BETWEEN WATER AND CHLOROFORM AT 35^
(Seidell, zgzoa.)
Gn. Cgi'
Gms. CnHaNA Recovered per zs cc:
Bfi Layer (a).
0.0006
O.OOIO
0.0021
0.0099
CHCU Layer (&) .
0.0I03(?)
0.0253
0.1299
0.6335
(«)
• • •
61
64
8TBTCHN1NE
688
8TBYCHNINB ABSSNATI CaHttNA.H,A804.iHsO(.iiH^).
100 gms. sat. solution in water contain 4.53 gms. ChHsNiOi-HiAsOa at 25*.
(Puckner and Wancn, i9xa)
100 gms. CHCla dissolve 0.085 gm. CnHaNiOi-HtAsOi at I5^ (HOI. 191a)
8TBTCHNIMX FOBMATE C11HttNA.HCOOH.2HsO.
Solubility in Watbr and in Alcohol.
CHampshire and Piatt, 19x3.)
Solubility in Water. Solubility in Abs. Alcohol.
r.
Gms. Salt per
zoo Gms. afi.
r.
Gms. Salt per
zoo Gms. QHiOH.
19s
30.59
18.5
10
24
39-68
20
10.3
27
44.25
22
10.64
8TBTCHNIN1 H7DBOBB01CIDS CkHttNAHBr.
100 CC HsO dissolve 1.54 gms. of the salt at I5*-20^ (Squire and Gaines, Z905.)
100 CC 90% alcohol dissolve 1.04 gm. of the salt at 15^-20®. ** "
8TBTCHNIMX HTDROCHLOBIDK CnHaNAHCl.
100 CC. HsO dissolve 2.86 gms. of the salt at 15^-20®. (Squire and Caines, Z905.)
100 CC. 90% alcohol dissolve i .37 gms. of the salt at i5*-20*.
100 gms. CHCU dissolve 0.592 gm. of the salt at 15 .
(Hill, Z9ZO.
STBTCHNIMX MITRATI CiiHssNA.HNO».
Solubility in Several Solvents.
Solvent.
Water
«
9o%CsHi0H
(I
100% CsHiOH
Solvent.
r.
CHsOH 25
CHCU 25
I vol CsHiOH+4 vols. CHCk 25
I vol. CsHiOH+4 vols. CdU 25
I vol. CHiOH+4 vols. CHCU 25
I vol. CHiOH+4 vob. CsH* 25
Glycerol 25
Gms. Salt
per zoocc.
Solvent.
0.34s
1. 25
5
0.66
4
I
1.66
Si
(z) Dott (z9zo); (2) Squire and Caines (Z905); (j) Schaefer (z9X3); (4) U. S. P. Vlll ed.
Distribution of Strychnine Nitrate between Water and Chloroform
Gms. CbH^A.HN(^
Added per xscc.
H^ + Z5 OC.CHCU.
0.005
0.025
0.125
0.625
AT 2S*»
(Seidell, 19x0a.)
Qam. CuHaNA-HNOb per 15 cc:
bfi Layer (a).
0.0051
0.0222
O.IOI7
0.3250
CHCU Layer (&).
0.0030 (?)
0.0042
0.0243
0.1698
a
b
5-3
4.2
2
8TBTCHNI1IX OXALATE
100 gms. H^ dissolve 1.13 gms. of the anhydrous salt at about 15^
a>ott, X9X0.)
8TBTCHNINE PEBCHLOBATE CsiHssNA.HC10«.
100 gms. HflO dissolve 0.022 gm. perchlorate at 15^
(Hoimann, Roth, HObold and Metskr, X9xa)
689 STRYCHNINE SULFATE
STRYCHNINE SULFATE (CtiHttNsOs),.H,S04.5H,0.
Solubility in Several Solvents.
Gms. Salt Gms. Salt
Sohpent. t*. per xoo cc Solvent. I*, per xoo cc
Solvent. Solvent.
Water 15-20 2.08(1) CHOi
' ■ u
" 2$ 3-23(2^
" 80 16.6 (2^ "
9o%CiHiOH 15-20 0.74(1) I vol. CiH»Om-4vols. CHCU
94% " 25 1.9 (2) I vol. CtHiOH+4 vols. CeH*
94% " 60 6.2 (2) I vol. CHiOH+4 vols. CHCli
100% " 25 0.8 (3) I vol. CHiOH+4 vob. CiH*
CH«OH 25 8.33(3) Glycerol
(x) Squire and Cainet (1905); (a) U. S. P. Vni; (3) Schaefer (1913); (4) HiU (19x0).
STRYCHNINE TARTRATE
Solubiuty op d, I AND OF Racbmic Strychnine Tartrate in Water.
(DutUh, X9X3.)
Gms. of Each Separately per xooo gma. ^0. ^
f.
tf Tartrate.
< Tartrate.
Racemic Tartrate.
7.35
14.14
9.48
14.02
16
17.72
11.50
19.12
as
22.9
14.52
24.70
27
• • •
15.60
• • •
30
• • •
17.02
• • •
40
35. 18
22.90
38.42
Solubility of Mixtures of d and / Tartrates and of Racemic Strychnine
Tartrate in Water.
(Ladenburg and Doctor, 1899.)
Results ford + l Tartrate.
Results for Racemic Tartrate.
Gms. Anhydrous
Gms. Anhydrous.
t*. Salt per xoo Gms.
Solid Phase.
r.
Salt per xoo Gms.
Solid Phase.
H/>.
H/).
7 I 48
So%rf+S%/
7
1.39
Saoemic Tartrate
19 1-95
u
19
1.90
<«
27 2.38
l<
27
2.33
K
35 302
(1
• 35
317
«
42 3-75
M
42
3.92
fl
100 gms. sat. solution in water contain 0.45 gm. anhydrous strychnine acid
tartrate at about 15^. (Dott, 1910.)
SUBERIC ACm C6Hit(C(X)H)i.
Solubility in Water.
(LamourouZf 1899.)
f. o*. IS*. 2o*. 35*. so*. 6s*.
Gms. CtHu(COOH)s per XOO CC. sol. 0.08 0.13 0.16 0.45 0.98 2.23
Solubility op Suberic Acid in Alcohols at 4**.
(TImofeiew, 1894.)
Gms. C|Hn(COOH)i per xoo Gms.
Alcohol. ^ - *-
Sat. Sol. Alcohol.
Methyl Alcohol 20 . 3 2 32 . 04
Ethyl Alcohol 15.5 18. 44
Propyl Alcohol 12.2 13 . 9
100 gms. 95 per cent formic acid dissolve 2.13 gms. CftHis(C(X)H)s at 19.5^
(Aschan, 19x3.)
Data for the distribution of suberic acid between water and ether at 25° are
given by Chandler, 1908.
SUCCINIC ACm 690
SUCCINIC ACm (CH,),(COOH)i.
Solubility in Water.
(MicqnBBki, x886; van der Stadt, 1902; Lamourouz, 1890; for other concordjuit resatU, see Bouxsiain*
1874; Henzy, 1884.)
Cms. Suocuuc
r.
Cms. (CH|)s(COOH)t per zoo
Gnu. Kfi. oc. Solution.
Anhydride
(CH4),C0C00
per 100 Cms.
Mol. Per cent.
H^.
(CHj^jCocoo:
HiO.
0
3.80
2.78 (L.)
2.34
99.58
0.42
10
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
^.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
19.9s
96.53
3.47
60
35-83
24. 5
28.77
95.07
4.93
70
51-07
• • •
40.11
93.26
6.74
80
70.79
54.08
91.12
8.88
89.4
95-45
70.62
88.71
11.29
104.8
146.3
IOI.2
84.57
15.43
115.1
188. s
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
t839
408. 5
57.6
42.4
182.8
00
542.3
50
50
174.4
• • •
808. s
40.7
59.3
153. 3
• • •
2239
19.86
80.14
128
• • •
8865.
5.89
94.11
118.8-119
• • •
00
0
100
The following very carefal determinations of the solubility of succinic acid
in water are given by Marshall and Bain (19 10).
t*. o*. xa.s*. as'- 37. S*. S©*. 6a. s*. 75*.
Gms. (CHj), (COOH),
perioo gms. H2O 2.75 4.92 8.35 14 23.83 3935 60.37
Solubility of Succtnic Acid in Aqueous Solutions of Salts and of
Acids at 25^
(Herz, i9zob, zgzz.)
In Aq. HBr.
In Aq. HCl.
In Aq. KBr.
In Aq.
KCl.
Gms. per Liter.
Gms. per Liter.
*-
Gms.
per Liter.
Gms. per Liter.
HBr. C4H«04.
HCl.
C4HA.
KBr.
C4IUO4.
KCl.
C4H^4.
0 81.21
18.45
66.25
0
81.21
28.34
75.58
79.3 57.38
45.6
50.78
65. 4!
; 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
502.1
62.59
267
61.41
In Aq. KI,
In Aq. LiCl.
In
Aq. NaCl.
Gms. per Liter.
Gms.
T.iCI.
per Liter.
C4H,04.
Gms. per
liter.
SoUd
KI. C4H,04.'
'NaCL
C4H.O4:
Phase.
0 81.21
0
81.
21
18.7
74.39
QHA
46.48 79.12
7.63
70.
86
32.73
69.68
i(
102.9 77.93
23.32
62.
59
64.3
61.41
«<
57.66
47-
24
132. 1
49.55
u
XI7
29.
51
289.4
27.16
<(
176.4
20.
07
315. 1
22.44
NaQ
231.5
14.
17
918
4.72
«
691
SUCCINIC Acm
Solubility of Succinic Acid in Aqueous Solutions of Potassium
Succinate and Vice Versa at Several Temperatures.
(Marshall and Cameron. 1907.)
Oms.per
xooGms.
Gin8.jper
100 Gms.
*•.
Sol.
Solid Phase.
f.
Sol.
^ Solid Phase.
KtCAO..
H,C4H404.
K,C4H404
•
0
2.71
0
HtCiHiO*
25
7.88
0
H,C4H404
0
7.26
8.09
" +KH,(C4H,04)t
25
9-965
3-17
(C
0
7.86
7.66
M it
25
12.77
8.4
((
0
8.24
9-95
KH,(QHi04),
25
17.6
14.15
«l
0
8. II
12,77
«i
25
18. 1
14.3
" +KH,(C4HAyt
0
7.87
15.47
" +KHC4HA.aH/)
25
15.36
18.48
KH,(C4H404),
0
0
40.2
E:,C4H«04.3H,0
25
13.7
23.6
" +KHC«H^4
14
1.468
41.3
KtCAOt+KHQHiO^
25
1306
23.81
KHC4H«04
+KHC«H«04.aH/>
25
11.98
24.43
M
15.9 1.7
34.36 KHC4H«04.3H|0+KHC«H|0
425
9.97
25
«<
20
6.39
0
HtCAOi
25
6.61
28.6
«(
20
7.48
1.8s
(1
25
2.6
38.2
M
20
14.63
11.64
««
25
2. II
40.6
C(
20
15.03
13.32
" +KH,(CA04),
25
1.03
48.7
" +K,C4H404.3HiO
20
13.32
18.46
KHiCQEiO^),
25
0.13
56.15
K«C4H404.3H^
20
12.74
22.45
" +KHC4H4O4
25
0
58.05
II
20
II. 7
22.91
KHC«H«0«
40
12.9
0
H,C4H404
20
1.71
42.1
i«
40
25.5
16.83
" +KH,(C4H404),
20
I. OS
47.3
" +K,C4H404.3H,0
40
19
25 . 48 KH,(C«EI«Q4),+KHC4H/)<
20
0.985
48.1
K,C4H404.3HiO
40
15.83
26.56
KHC4H/)4
20
0.909
48.75
w
40
0
62.10
K^:W>4'SBfi
20
O.IS9
54. 3
M
20
0
56.6
<l
Solubility of Succinic Acid in Alcohols and in Ether.
(Timofeiew, 1891, 1S94; at 15% Bouzsoin, 1878.)
S<dvent.
Abs. Methyl Alcohol
Abs. Ethyl
90% "
Abs. Propyl
Abs. Ether
Isobutyl Alcohol
Gms. (CH|)t(COOH)s per 100 Gms. Solvent at:
tt
«
-!•.
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
100 gms, 95 per cent formic acid diasolve 2.06 gms. (CHs)2(C00H)s at 18.5^.
(Aschan, 19x3.)
Distribution of Succinic Acid between Water and Amyl Alcohol
AT 20'*.
(Herz and Fischer, 1904.)
Mmimob iC«H^4
per xo cc.
Gms. C4HA
per xoocc.
MflUmob iC4Hd04
per 10 cc. ^
Gms. C4H^4
per xoo cc.
Alcohol Aq.
Laytt. Layer.
0.1888 0.2684
0.3643 0.5252
0.7077 1.0373
1.440 2.1266
2.715 4.0495
' Alcohol Aq.
Layer. Layer.
O.III4 0.1584
0.215 0.310
0.418 0.612
0.850 1.255
1.603 2.391
Alcohol
Layer.
3.899
5.199
6.334
7. 119
Aq.
Layer.
6.0795
8.099
10.170
".555
Alcohol Aq.
Layer. Layer.
2.302 3.588
3.069 4.779
3.739 6
4.202 6.821
SUCCINIO Acm
692
Solubility of Succinic Acid in Aqueous Acetone at 20®.
(Hen and Knoch. 1904.)
oc. Acetone per
xoa|oc. Soltttioo.
O
10
30
30
40
SO
C|H/)4 per lop cc. Solution.
MiUimols. Cms.
107.8 6.363
127.4 7.519
iss-^ 9194
186.7 11.02
"54 1330
254.3 IS 01
cc. Acetone per
100 cc. Solution.
60
70
80
C|H/>i per 100 cc Solutioo.
MiUimols.
27s. 7
278. s
265.3
201.9
51. S
Gms.
16.27
16.44
15-66
II. 91
304
Solubility of SucaNic Acid in Aqueous Glycerol S(h.utions at 25*.
CHers ind Enoch, 1905.)
Wt. %
GJ^oerolin
Solvent.
O
7.15
20.44
31. S5
C|H^< par zoo cc.
Solution.
Millimolsr
133.4
128.2
118. 3
109.7
Gnu.
7.874
7.566
6.982
6.476
Sp. Gr. of
Solutions.
1. 0213
1.0407
1.0644
1.0897
Wt. %
Glyceruin
Solvent.
40.9s
48.70
69.20
100*
CfHjPf per zoo cc.
Solution.
MiUimols.
105.8
99.9
88.5
74.6
Gms.
6.244
S.896
S-223
4.440
Sp. Gr. off
Solutions.
I.II20
I. 1298
I. 1804
1.2530
* Sp. Gr. of Glycerol » i,asS5- Impurity about z.5 per cent.
Distribution of Sucamc Acid between Water and Ether at 15®, 20*
AND 25.5*.
(Pinnow, 19x5.)
Results at is"*.
Gm. M0I&. per Liter.
Results at 20^
Gm. Mob. per Liter.
Aqueous Ether ' p*
Layer (e). Layer (c*).
0.644 0.096 6.71
0.312 0.046 6.87
O.151 0.0218 6.93
Results at 25.5^
Gm. Mols. per Liter.
Aqueous Ether p'
Layer (c). Layer (O*
0.474 0.0783 6.05
0.2585 0.0415 6.23
O.II75 0.0187 6.28
Aqueous Ether p*
Layer (c). Layer (cO-
0.3293 0.0438 7.52
0.1768 0.0235 7.52
0.0894 O.OI16 7.71
0.0405 0.006 6.75
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
y Kolossovsky, loii. Earlier data for this system are given by Nernst, "Theo-
retical Chemistry, 3rd English edition, p. 496.
BromSUCCINIC ACID CHBr(CH,)(COOH), (m. pt. 159**).
SOLUBILITT IN ALCOHOLS AT 22®.
(Timofeiew, Z894.)
Alcohol.
Gms. CHBr(CH^(C00H)9 per zoo Gms.
-JL.
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 +1 Chlorsuccinic Acid.
d-i-i Chlorsuccinic Acid.
d Chlorsuccinic Acid + 1 Bromsuccinic Acid.
i Chlorsuccinic Acid + 1 Bromsuccinic Acid.
d-^-l Benzylaminosuccinic Acid.
d-jri Aminosucclnic Acid.
693
8UCCINIMIDE
8UCCINIMIDE CH4<^g>NH.
Solubility in Water and in Ethyl Alcohol.
Interpolated from original results.
In Water.
f.
Wt.o£
r cc.
Solution.
MQls.jper
zoo Mob.
H,Q.
o
1.025
1.58
lo
1.03s
2.4
20
25
30
1.052
1.067
1.086
4
59
8
4P
1. 120
12.8
SO
60
1. 145
1. 167
17.8
22.6
70
80
1. 189
1.204
27. 5
32.8
ts.
(Sp^yen, 1903.)
In Ethyl Alcohol.
Gms. per
Wt.o£
Mob-per
looMols.
Gins, pcf
zoo Gins.
I cc.
zooGms
H/).
Solution.
QHtOIL
CAOH
8.69
0.815
0.88
1.89
14
0.809
1-35
2.7
23
0.806
2
4.1
33
0.805
2.5
5-3
45
0.804
3.1
6.8
70
0.809
4.9
10.5
96
0.816
7.8
16
124
0.835
12.3%
26.5
152
0.873
• • •
• • •
• « •
0.954
• • •
• • •
^ Freezing-point data (solubilities, see footnote^ p. i), are given for ethylsuc-
cinimide + bromotoluene and for ethylsuccinimide + p xylene by Patemo and
Ampola (1897).
SUCCINIC NITBILE (Ethylene Cyanide) CNCH,CH,CN.
The solubility of succinic nitrile in water and also in aqueous sodium chloride
solutions at various temperatures has been determined by bchreinemakers (1897),
and the results presented in terms of mols. of nitrile per 100 mols. of nitrile + H jO.
The following calculations of these results to gram quantities was made by
Rothmund. (Landolt and BOrnstein's, " Tabellen " 1906.)
♦•
Gms. CNCH«CH«CN per 100 Gms.
Gms. CNCH^C^CN per zoo Gms
Aq. Lsytt.
Nitrile Layer.
Aq. Lajrer. Nitrile Layer.
18.5
10.2
92
53-5 33.2 66.4
20
II
91.5
55 40.3 6a. 8
39
• • •
85.2
55.4 ciit. temp. 51
45
22
• • •
Very complete data for the sj^tem succinic acid nitrile, ethyl alcohol and
water, determined by the synthetic sealed-tube method, are given by Schreine-
makers (i8p8c). Results for the system succinic acid nitrile, cane sugar and
water are given by Timmermans (1907).
SUGAB CuHttOii (Cane Sugar.)
Solubility in Water.
(Hersfeld, zSga; see also Courtonne, Z877.)
Gms. CaHiAi iwr
Gms. CbB^Ai per
r.
zoo
Gms.
f.
zoo
Gms.
Solution.
Water.
&>lution.
Water.
0
64.18
179.2
40
70.42
238.1
5
64.87
184.7
45
71.32
248.7
10
65.58
190.5
50
72.25
260.4
15
66.33
197
60
74.18
287.3
20
67.09
203.9
70
76.22
320.4
25
67.89
211. 4
80
78.36
362.1
30
68.70
219.5
90
80.61
415.7
35
69.55
228.4
100
82.97
487.2
'© ^
» I
.M
o.
Sp. Gr. of sat. solution at 15** =» 1.329; at 25*
100 gms. H|0 dissolve 212 gms. cane sugar at 25^, determined by means of
Pulfrich's refractometer. (Osaka, zgos-os.)
SUGAR 694
Solubility of Sugar in Aqueous Salt Solutions at 30®, 50**, and 70*.
terpc
>lated from ori
ginalreau
ilts.
(Schukow, 1900.)
f.
Gms. Saltper
zoo Gms. £uO.
Gms. CisHaOu
per xoo grams
HsO in Aq. Solutkn of:
KQ.
KBr.
KNQt.
Naa.
Cads.
30
0
219s
2195
219s
219s
219.5
€€
ID
216
218
217
aio
197
U
20
221
220
216
211
189
it
30
228
224
216
219
192
u
40
237
228
217
233
200
it
50
■ • •
• • •
218
250
218
u
60
• • •
• • •
• • •
269
243
50
0
260.4
260.4
260.4
260.4
260.4
ik
• 10
261
262
260
255
239
it
20
266
266
261
260
228
u
30
274
.272
262
269
228
u
40
284
276
262
284
236
a
50
296
280
263
302
253
t€
60
■ • •
• • •
• • •
• • •
276
10
0
320.5
320.5
320.5
320.5
320.5
If
10
326
324
321
323
295
M
20
334
328
324
330
286
4%
30
345
334
327
344
286
II
40
357
341
33^
361
295
u
SO
370
349
334
384
308
u
60
384
357
337
406
327
Solubility of Cane Sugar in Saturated Aqueous Salt S(X.utions at
31.25^ (Ktthler. X897.)
Gms. Sugar per zoo Gms. „ ,. Gms. Sugar per xooGsds.
daii.
Soltttiaa.
Water.
CHjCOOK
. • •
324.8
C,H,COOK
49.19
306.1
C,H«.OH.(COOK),
50-30
303 -9
KjCO,
56.0
265.4
KCl
62.28
246.5
CHjCOONa
59-93
237.6
NaCl
62.17
236.3
aaic.
Solution.
Water.
Na,CO,
64.73
229.2
KNO,
61.36
224.7
K^O*
66.74
219.0
CHjCOOCa
60.12
190.0
Na,SO«
52.20
183-7
CaCl,
42.84
135 -I
MgSO«
46.52
119. 6
Solubility of Cane Sugar in Aqueous Alcohol Solutions at 14®*
(Schiefeld, 1894.)
Wt.
Wt.
per cent
Alcohol.
O
5
10
20
30
40
Wt.
per cent
Sugar.
66.2
64.25
62.20
58-55
54 -OS
47-75
Gms. S
GC. Alcohol-UsO
Mixture.
X per zoo
195.8
179.7
164.5
141. 2
117. 8
91.
Wt. Gms. Sugar per 100
per cent per cent cc. Alcohol-HjO
Alcohol. Sugar. Mixture.
50 3855 <52.7
60 26.70 36.4
70 12.25 13-9
80 4.05 4.2
90 0.95 , 0.9
100 c.oo ' 0.0
695
SUQAB
Solubility of Cane Sugar in Aqueous Alcohol Solutions.
(Scheibler, 1872; correction, 1891.)
Results at 0"".
Results
at 14**.
Results
at 40**.
Percent
Alcohol
byVoL
Sp. Gr. of
Solution at
17.5'.
Gms. Sugar
■Sp. Gr. of
Gms.
per 100 cc. J
Solution.
Gnu. Sugar
per luu cc.
Solution.
OUiUUUii Ac
17-S'-
Sugar.
C,H,OH.
0
H,0.
per luu cc
Solution.
0
1325
85.8
1.326
87.5
45. 10
a a *
10
1.299
80.7
1.300
81.5
3.91
44.82
95.4
20
1.236
74.2
1.266
74.5
8.52
43.83
90
30
1.229
65.5
1.233
67.9
13.74
41.87
82.2
40
1. 182
56.7
I. 185
58
20.24
40.38
74.9
50
1. 129
45. 9
I. 131
47.1
28.13
38.02
63.4
60
1.050
32.9
1.058
33.9
37.64
34.47
49-9
70
0.972
l8.2
0.975
18.8
46.28
29.57
31.4
80
0.893
6.4
0.895
6.6
61.15
21.95
13.3
90
0.837
0.7
0.838
0.9
71.18
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.)
Sp. Gr. of
Solutions.
1.3306
1.2796
I . 2491
1.2002
I.1613
Solubility of Cane Sugar in Aqueous Acetone at 25**.
(Herz and Enoch, 1904.)
Gms. Sugar
per 100 cc.
Solution.
89.8
76.7
cc. Acetone
per 100 cc
Solvent.
O
20
30
40
45
72.1
59.3
52.5
Gms. per zoo cc.
Solution.
H,0. (CHOiCO.
CuHaOu.
43-3 0
89.8
42.9 8.4
76.7
39.5 13.4
72.1
39.8 20.9
59.3
39 24.6
52.5
Above 45 cc. acetone F>er 100 cc. solvent the solution begins to separate into
two layers. The lower of these contains si gms. sugar p>er 100 cc. and has Sp.
Gr. 1. 1 522. 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.
Solubility of Several Sugars in Pyridine at 26®.
(Holty, 1905.)
Gms. Sugar
Sugar.
Cane Sugar (Sucrose)
Milk Sugar (Lactose)
Grape Sugar (Glucose)
Fruit Sugar (Fructose)
Galactose
Maltose »
Maimose
Raffinose
* It is uncertain whether these figures refer to gms. per xoo gms. sat. solution or gms. per xoo gma.
pyridine at 20*-2S*.
100 gms. aq. 50 per cent pyridine dissolve the following g^s. 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.)
loogms. 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.
Foimula.
da of Sat. Sol.
per xoo Gms.
Sat. Sol.
CnHfcO,!
• • «
6.45
CttHBOu.H,0
0.981
2.18
J(VHjsQ,.H^
1.005
7.62
/CtHnOi
1.052
18.49+
CVHaO,
1.0065
5.45(?)
CbHbOu
• • •
98.10*
(Dehn, 1917.)
C.HaO,
• • •
29.9*
M
CttH«0,..sHiO
• ■ •
75*
U
SnOABS
696
Solubility of Milk Sugar (Lactose) Hydratb and /3 Anhydridb 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 ec^uilibrium and that the mutarotation of
milk-sugar results from the slow establishment, in cold solutions, of the equi-
librium of the balanced reaction, CisHtiOu (Hydrate) ^ H|0 -|- CuHitOu 09-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 fi anhydrides, weighed.
f.
Gms. CttH^^u
per xoo Gms.
Sat. Sol
■
Gms. CuHtfOu
per zoo Gms.
Sat. SoL
0
10.6
49
29.8
IS
25
39
14. s
17.8
24
64
74
89
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 fi 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 NH4OH
solution. At o^, 42.9 gms. CuHttOn per 100 gms. sat. solution were found and
at 100^, 61.2 gms.
Solubility of Several Sugars in Aqueous Alcohol at 20*.
(Hudson and Yanovsky, 191 7.)
Sugar.
a Aiabinose
fiCeJlose
fi Fructose
p "
a Galactose
(C
pj a Glucoheptose
a Glucose
a "
a " hydrate
p Glucose
a Lactose hydrate
aLyxose
p Maltose hydrate
P Mannose
p "
P Mellibose Dihydrate
a Rhamnose Hydrate
a " "
a Xylose
Sucrose
Trehalose Dihydrate
Raffinose Pentahydrate
Formula.
CuHaOu
QHiA
<«
«<
II
QHiA
CiHaO,
II
CHaO,.H,0
C|Hu0«.
CnHa0ii.H,O
CiHuOfe
CuHbOu.H,0
C^HttO,
41
CuHaOi.aH^
CHiA-HjO
II
C,H«A
CuHbOu
CisH«0u.2H,0
CuHaOu.5H^
Solvent.
u
ti
8o%CiHiOH
20%
80%
95%
Methyl Alcohol
6o%CtHiOH
80% "
20% "
80% «
Methyl Alcohol
80% COIiOH
80%
40%
90%
60%
80%
Methyl Alcohol
80% CjHjOH
100%
70%
80%
80%
70%
tt
it
tt
it
tt
(C
«
tt
tt
Gms. Anhydrous Sugar
per 100 cc. Solution.
Initial
Solubility.
Final '
Solubility.
0.74
1.94
3-2
4.7
13.4
27.4
1.8
4.2
5-2
II. I
I.I
3.1
0.27
0.65
4
45
2
0.8s
4-5
1.6
1.3
3
4.9
9.1
I.I
2.4
5-i
7.9
3*
4.7s
2.4
0.78
0.76
8.6
8.2
13
4.4
1-3
95
9.6
2.7
6.2
3-7
1.8
3.7
1.8
1.4
1.4
697
SnOABS
Solubility of Sorbose and Gulosb in Water and Alcohols.
(de Bruyn and van Ekereitcin, 1900.)
Sugar.
d Sorbose
I Sorbose
/ Gulose
M.-pt.
151
ISO
ISO
Cms. Sugar per xoo cc. Sat. Sol. in:
H^ at 100".
0.22
0.23
0.24
100 gms. HiO dissolve 108 gms. maltose at 20^-25^.
100 gms, HsO dissolve 14.3 gms. raffinose at 20^-25^
CH/DH at 17*
1.70
1.68
1.72
CaH»0H at 17".
1.02
I
1.04
(Dehn, xgzr.)
Solubility of Phenylhydrazones and fi Naphthylhydrazonbs of the
Sugars in Water and in Alcohols at i6°-i8®.
(van Ekenstem 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 recrystalliz^
from 30 to 50 per cent alcohol. No details in r^;ard to the method of obtaining
saturation or of analysis of the solutions are given.
Gms. Compound per xoo oc. Sat. Sol. in:
Phenylhydxasone of:
M.-pt.
Water.
CHjOH.
CAOH.
Methyl Mannose
178
0.2-0.06
0.59
0.05-0.02
" Arabinose
161
(i
• « •
u
" Rhamnose
124
u
very si. sol.
«
" Galactose
z8o
(t
u
M
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
Z20
• • •
3-6
" Rhamnose
99
very si. sol.
6.5
" Glucose
128
• ■ ■
Z.2
" Lactose
123
• « •
0.4
Allyl Galactose
IS7
• • •
0.3
" Mannose
142
• • •
0.7
" Arabinose
I4S
• • m
o.S
'< Rhamnose
135
% • •
• • •
" Glucose
^SS
• • 9
• • •
" Lactose
132
• • •
0.2
" MeHbose
192
• • •
0.3
Benzyl. Galactose
154
. 0.9
0.08
" Mannose
i6s
0.5s
0.2
" Arabinose
170
0.4
0.06
" Rhamnose
121
iS-4
6.7
" Glucose
150
OS
O.IO
" Lactose
128
0.9
0.06
fi Naphthyl Galactose
167
0
■14
...
0.24*
" Mannose
157
0
.18
...
0.25*
" Arabinose
141
0
.22
...
0.62*
*' Rhanmose
170
0
.20
...
0.44*
" Glucose
95
0
•25
...
5*
Xylose
70
0
•32
...
6.62*
" Lactose
203
0
.07
...
0.2*
« Maltose
176
■ • •
a . .
0.4*
'' MeUbose
13s
• « •
• • •
1.3*
* Solvent 96 per cent CiH^H.
SnOABS
698
Sqlubility of thb Bbnzalic Compounds of Somb Polyatomic Alcohols
AT I6^-I8^
(de Brayn and van Ekmrtein, 1899.)
No details of the determinations are given. . It is stated that the results are
sufficiently exact for use in identifying hexites.
Cms. Compd. Dbaolved pei
' zoooc
Name of CompoiuuL
M.-|it
aai. :>oi. in:
r
Acetone.
Chloroform.
AkohoL
Dibenzalerjrthritol
SOI
(Fiicfaer)
0.34
364
0.02
Monobenzalarabitol
152
ii
• * •
• • *
• • •
Dibenzaladonitol
165
«(
0.64
1.36
0.14
Dibenzalxyiitol
175
«(
1. 10
0.85
« • >
Dibenzalrham nitol
203
i<
0.70
2-55
1. 10
Monobenzal-<i-Sorbitol
175
(Meunier)
very
easily soluble
Dibenzal-(i-Sorbitol
163
<t
5-44
0.16
O.IO
Tribenzalmannitol
213-8
(Fiflcher)
0.42
8.75
O.IO
Trihenzal-^iditol*
215-8
u
0.47
0.17
0.05
Tribenzal-<f-taJitoit
210
Ii
0.30
4.42
trace
Dibenzalduldtol
215-20
(f
0.42
0.83
trace
Dibenzalperseitol
230-5
u
0.04
trace
0.02
* Prepared (rom / idonic add.
t PrepaP
ed from d talonic add.
100 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^. "
SULTAlinJC ACID NH,.C«H4.S0sH.H,0.
Solubility in Water.
(Philip, 19x3; lesults for 60* and over by Dolinski, 1905.)
Gms. NIL.-
Gms. NIL.-
f.
per 100 Gms.
Solid Phase.
f.
pS'^fJm, SoKd Phase.
SatSd.
Sat.SoL
0
0.444
NH^.C|H«.S0|H.aH^
44
2.44
NHt.C»H,.SO,H.H/)
7.2
0.622
«
44
2.36
NH|.CA.S0^
13-3
0.841
<i
47-5
2.52
<(
18.9
1.093
((
54.5
2.8s
((
18.9
1. 137
NH,.CA.S0»H.H^
60
301
u
25.1
1.384
K
70
3.65
u
31.1
1.662
H
80
4.32
«
37.2
2.004
U
100
6.26
u
SULTONIUM PEBCHL0RATE8
Solubility in Water.
(Hofmann, Hdbold and Quoos, 1911-1 a.)
Name.
Formula.
f.
Per TOO Gms. H^.
Gm. Mols.
- Gms.
Trimethyl
Sulfine
Perchlorate (CH^jSCio*
16.5
0.0784
13.84
Ethyl dimethyl
u
CH,(CHOiSC104
15-9
O.II91
22.31
Propyl
«
C,H7(CH,),SC104
IS
0.0590
12.04
n Butyl "
it
C4H,(CHa),Sa04
IS
0.0607
13.24
Ethylene dt^methyl
•
<c
C,H4(C,H«SC104),
18
0.0423
14.86
Vinyl dimethyl
<(
Q,H|.S(CH,),.C104
18
0.0731
13. 75
Trimethylene dismethyi "
•
C«H,:(QH«Sa04)s
18
0.0402
14.68
699
TriethylSULTONIXTM IODIDE S(CsH»)sI.
lOO gms. HiO dissolve 431 gms. S(CjH*)»I at 25*.
100 gms. CHCli dissolve 47.7 gms. S(CsH6)iI at 25*
SULTONIUM IODIDE
(Peddle and Turner, 19x3.)
(Peddle and Turner, 19x3.)
SULFUB S.
In a series of papers by Aten (1905-06, 1912, 1912-13, 1913, 1914 and 1914a),
the preparation and properties of the four known modifications of sulfur are de-
scribed. These are oesig^ted by the symbols, Sx, S/i, Sr and Sp.
Sx is ordinary rhombic sulfur and its molecule is considered to be composed of
eight atoms of sulfur, Sg.
Sn is the insoluble, so-called amorphous sulfur.
sir is obtained when ordinary sulfur is heated above its meltine-point and
?[uickly cooled; it is especially easily prepared by warming Sx in sulfur chloride,
ts molecule is probably represented by S4.
So was discovered by Engel and is prepared by mixing concentrated HCl,
cooled to o^, with saturate 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 Se.
Solubility of Sulfur (Sx) in Sulfur Monochloride (SsCk) Determined
BY THE Melting-point Method.
(Aten, X905-06.)
f of Melting.
-16
O
+ 17.9
36.8
55.2
65.6
77.7
Mol. % Ss in
Mixture.
4-3
6
9.9
17. 1
28.5
40.3
55. (^
Solid Phase.
t* of Melting.
Rhombic S
835
95.6
86
103.2
IIO.4
118. 8
Mol. % S« in
Mixture.
Solid Phase.
67
Rhombic S
81.8
«(
81.8
MonodinicS
88.4
u
95
(i
100
(i
Solubility of Sulfur (Sf) in Sulfur Monochloride (SaCli)
(Aten, X9ia-i3.)
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 SsClt in tubes, heating them to 100^ for
several hours and then cooling quickly to the indicated temperatures and shak-
ing for i hour in the case of the 0° and 25** results and 2 hours in the case of the
—60** results. The saturated solutions were analyzed by oxidizing with HCl
+ HNOi + Br and titrating the HsSOi, after removing the volatile acids.
Atoms S
per xoo Atoms S+SiQs
in:
Atoms S
) per xoo
Atoms S+SiCl,
urated Solution
tin:
Original
Saturated Solution at:
Original
Mixture.
Sat
at:
Mixture.
-6o-.
o*.
+as-. '
-eo".
o*.
+2S".'
0
II. 6
36.1
53.5
79.4
65.2
72
• • •
10
18. 1
40.1
57.6
Ik). 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. s
• • •
60.1
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, 19 12), for mixtures previ-
ously heated to 50®, 75** and 125**. All the data confirm the formation of the
the new modification Sr>
SULFUB
700
Solubility of Sulfur (S,) in Sulfur Monochloridb (SiCls) at 25*.
(Aten, 191a, 1913)
The samples were heated to the temperatures indicated and rapidly cooled
and powdered. The method of determining the solubilities is not described.
Previous Treatment of Sample.
Unheated Sulfur
Mixture of Rhombic and Amorphous
Sulfur
Rhombic Sulfur heated to 125^
" " " " 165**
" " " " i6s**
" " " " 165**
a u a a ^^^o
Atoms S Dis-
solved per 100
Atoms d+S|Gt<
53-5
54.5
56-58 . 5 (depending on excess of S pieaent.)
60 (determined immediately.)
59. 5 " after I hr.)
57.5 " « 24 h».)
53.2 " " 8 days.)
Solubility of Sulfur (S,) in Toluene at o* and at 25*.
(Aten, 1913)
Comp. of Mix-
ture in Atom
Per cent S.
35
47
54
57
73
Sdubility in Atom % S.
Ato*.
3.88
• • •
3.26
3 30
At as*.
S-94
6.6s
6.76
6.88
7.4s
Comp. of Mix-
ture in Atom
Per cent S.
74
77
80
83
85
Solubility in Atom % S.
Ato*.
40s
3
4
At as*-
7. 52
90
22
7
8
93
08
These results show that the greater the excess of Sr, 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
Sx was found and at 25**, 5.65 atom per cent.
Solubility of Sulfur (S^) in Carbon Disulfide and Carbon
TETRACm^ORIDB.
(Wigand, 1910.)
When "insoluble" sulfur {SsJ) is treated with CSs or CCU, a small amount
dissolves, depending upon the lenc^th 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 S^ to soluble sulfur
Sxi takes place.
Data for the fusion points of mixtures of rhombic sulfur and "insoluble"
sulfur (S|i) and for monoclinic sulfur and "insoluble" sulfur (Sj«) are given by
Kruyt (1908).
Solubility of Sulfur in Liquid Ammonia.
(Ruff and Hecht, 191 x.)
At the temperatures o^ to 40^, the solutions were constantly shaken for 3 to ^
days. For the results at the lower temperatures the solutions were saturatea
at room temperature then cooled, partial^ 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 lOO**, with proper precautions, and
weighed.
t*.
78
20. s
o
Gms. S per xoo Cms.
Sat. Solution.
38.6*
38.1*
32.34
+ 16.4
30
40
Gms. S per zoo Gms.
Sat. Solution.
25-65
21
18. 5
This figure corresponds to the compound S(NHa}| "■ 38.5% S.
701
SULFUR
SOLUBILITT OF SULFUR IN AqUBOUS SODIUM SULFIDE SOLUTIONS.
(KQster and Heberlein, 1905.)
The results are expressed in terms of x which represents the number of S
atoms dissolved for each Nat in the solution. The figures, therefore, show the
atomic ratio of S to Nat in the saturated solution and at the same time, the sulfur
content of the compound Nas3c 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 equilibnum 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.
Na«S Solution.
4
2 (2 hrs.)
I
OS
0.25
X in the Result-
ing NatS..
4
4
4
S
47S
666
84s
984
NOTmality of the Aq.
Na^S Solution.
0.125 (32 hrs.)
0.0625
0.03125
0.015625
0.007812 (128 hrs.)
« in the Result-
ing Na^S,.
s
s
s
s
4
225
239
198
034
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 NaiS 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 NatS 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.
(Geiardin, i
B6s.)
(Geiardin.)
99
Gms. S
per 100 Gms.
SnCU.
S.8
.Solid
Phase.
Solid S
95
Gms. S
per 100 Gms.
CiHuOH.
1.5 S
lOI
6.2
«
no
2 . 1-2 . a
no
8.7-9.1
«
iia
2.6-2.7 I
112
9.4-9.9
Liquid S
120
30
121
17.0
«
131
S'3
Solid
Phase.
SoHdS
Liquid S
It
Solubility of Sulfur in Aqueous Acbtonb at 25**.
(Herz and Knoch, 1905.)
Wt. Per cent
Acetone
in Solvent.
100
95-36
90.62
85.38
Sulfur per 100 cc. Solution.
65
4S
33
25-3
Gms.
2.084
1.442
1.058
O.81I
Sp. Gr. of
Solution.
0.7854
O.7911
0.8165
0.8295
8UL7I7B
702
SoLUBiLrrY OF Sulfur in Ethyl and Methyl Alcohols.
IS
18.5
b. pt.
18.5
Alcohol.
Abs. Ethyl
u
«
Abs. Methyl
Gms.
per 100 Gms.
Alcohol.
0.051
0053
0.42
0-028
Authority.
(Pohl.)
(de Bruyn — Z. physik. Oiein. xo» 781, 'gm^
(Paycn — CompC. rend. 34* 356. '52.)
(de Bruyn^
Solubility of Sulfur in Benzene and in Ethylene Dibromidb.
(Etard, 1894; aee also Coua, 1868.)
In C.H..
In CH^Br,.
Gms. S
t*. per xoo Gms.
SolutioD.
O
10
20
25
30
40
50
60
I.O
1-3
1-7
2.1
2.4
3-2
4-3
6.0
Gms. S
t^. per xoo Gms.
Solution.
70 8.0
80 10. 5
90 13.8
100 17.5
iio 23.0
120 29.0
130 36.0
O
10
20
25
30
40
Gms. S
per 100 Gms.
Solution.
1.2
1-7
2
2
3
4
3
.8
3
4
Gms. S
t*. per xoo Gms.
Sojutian.
50 6.4
60 8.4
70 II. 4
80 16.5
90 24.0
106 36.5
RsaPROCAL Solubility of Sulfur and Benzene, Determined by thb
Synthetic Method.
(Kruyt, 1908-09.)
Wt. % S in I«imiting t* of ^Homogeneity.
Mixture. Lower. Upper.
41 . 5 146 247
55-2 158 230
74-5 157 226
Wt. % S in
Mixture.
79.8
81.4
83.4
Limiting t* of Homogeneity.
Lower. Upper.
141 230
138 above 246
131 " 272
100 gms. sat. solution of S in benzoyl chloride, CsH«.COCi, contain i gm. S at
o" and 55.8 gms. at 134®. (Bogousky, 1905.)
Solubility of Octohedral and of Prismatic Sulfur in Several Solvents.
(BrOnsted, 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.
*tn1v»nt'
f.
18.6
Gms. each Variety Separately per
xoo cc. Saturated Solution.
Benzene
Prismatic Octohedral'
Sulfur. Sulfur.
2.004 I. 512
Chloroform
25.3
0
2.335 1.835
I.IOI 0.788
((
15.5
1.658 1.253
Ethyl Ether
40
0
2.9 2.4
O.II3 0.080
Ethyl Bromide
Ethyl Formate
Ethyl Alcohol
253
0
253
0
25.3
0.253 0.200
0.852 O.61I
1 . 676 1 . 307
0.028 0.019
0.066 0.052
703
SULFUB
S(X«UBILITY OF SULTUR IN SEVERAL SOLVENTS.
Sohrent.
Aniline
Benzene
t»
<t
It
19-3
26
TI
Carbon Tetrachloride 25
Chloroform
tt
it
Dichlor Ethylene
Ethylene Chloride
Ethyl Ether
Gin8.S
t**. per 100 Gms.
Solvent.
130 85.3 (l
15.2 i.s (2
1.7 (2
0.97(1
4.38(1
0.86(3
12.2 0.75(2
19.3 0.92(2
22 1.21(1
25 1.28(3
25 0.84(3
23.5 0.97(1
Gms. S
Solvent. t". per 100 Gms.
Solvent.
Glycerol 15.5 o . 14 (4)
Hydrazine (anhy.) room temp. 54(<^l<eamip.)(5)
Lanoline (anhy.)
Methylene Iodide
Nicotine
Phenol
Pentachlor Ethane
Toluene
Tetradilor Ethane
Tetrachlor Ethylene 25
Trichlor Ethylene 25
15
45
10
100
174
25
23
25
(t
0.38(6)
10 (7)
10.6 (8)
16.4 (i)
1.2 (3)
1.48(1)
I • 23 (3)
1.53(3)
1.63(3)
1 . 16(9)
(x) Coasa, x868; (a) Br6n8ted, i9o6: (3) Hoffman. Kirmreuther and ThaL 19x0; (4) Osaendowski, 2907:
g;) Welsh and Broderaon, 19x5; (0) ^lose, 1907; (7) Retgen» X893; (8) &kven, x87a; (9) Wester ana
rains, 1914.
SoLUBn^rrr of Sulfur in Carbon Disulfide.
(Etaxd, 1894; Coisa, 1865; at xo% Retgecs, 1893; below 77*, Arctowski, 1895-96.)
^^ Gms. S pe
r zoo Gms.
cs.
t».
Gms. S per zoo Gms.
Soludon. CS3.
e Gms. S pa> zoo Gms.
Solttdoo.
* Solutioa. CSs. '
— iio 3.0
31
-ID
13 5
15.6
SO 59.0 143.9
-100 3.5
3-6
0
18.0
22.0
60 66.0 194. I
— 80 4-0
4-3
ID
23 0*
29.9
70 72.0 257.1
- 60 3.5
3-6
20
29s
41.8
80 79.0 376.1
— 40 6.0
6.4
25
33-5
50.4
90 86.0 614. I
— 20 10.5
II. 7
30
38 0
61.3
100 92.0 II50.O
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 Hbxanb (QHw).
(Etard.)
Ao Gms. S per
* * zoo Gms. Solutioa.
" ' zoo Gms. SoludoQ.
Ao Gms. S per
zoo Gms. Solatka.
— 20
0.07
60
1.0
130 5.2
0
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 fi Naphthol, Dbtbrminbd by thb
Synthetic Method.
(Smith, Holmes and Hall, Z905.)
The mixtures of sulfur and p naphthol were heated until they were homo-
geneous and then cooled to the temperature at which clouding appeared.
f of
Clouding.
Gms. S
per zoo Gms.
0 Naphthol.
f of
Oouding.
Gms. S
per zoo Gms.
^Naphthol.
fof
Clouding.
Gms. S
per 100 Gms.
0 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
II9-3
163.8
264.8*
143.5
59.3
162.5
145. 1
163
300 •
149.5
70
163.5
177.6
* Solid phase, 0 naphthol.
SULFUR
704
Solubility of Sulfur in Coal Tar Oil, Linsbbd Oil and in Olivb Oil.
(Pdouse, Z869; PoU.)
wnuns 0
per 100 01
VDS \AMX
iBT v/u cx:
G. Sper
TOO Gms.
«• Sp.Gr.
• • b. pt.:
8o».ioo».
0.88
oJ»J
iao*-aao*.
0.88s
i50«-air
I4>I
, no*-300*.
XjOS
aao'-joo*.
»S
2.1
2-3
2-5
2.6
6.0
7.0
0.4
23
30
30
4.0
5-3
5-8
8s
8-5
0.6
4.3
SO
5-2
6.1
8-3
8.7
10. 0
12.0
1.2
90
80
II. 8
137
15-2
21.0
37 0
41 -o
2.2
18.0
100
iS-2
18.7
23 0
26.4
52 S
54 0
30
25.0
no
• • •
33.0
26.3
31 0
105.0
115 0
3-5
30 0
I30
• • •
37.0
32-0
38 0
00
00
4.2
37 0
130
• • •
• • •
38 -7
43-8
00
00
(i6o<»)
50
10 .0
43 0
100 gmt. oil of turpentine dissolve 1.35 gms. S at i6^ and 16.2 gms. at b. pt.
(Payen, 1853.)
Solubility of Sulfur in Triphbnyl Methane, Determined by the
Synthetic Method.
Results of Smith, Holmes & Hall, 1905. Results of Krujrt, 1908-09.
Mixture.
69.1
t*of Fim
Limit of
Mixing.
108. s
% Triphenyl t* of Second
Methane in Limit of
Mixture. Mixing.
35.5 214.5
%Triphei^l
Metiikne m
Mixture.
66.7
t* of Pint
Limit of
Mixing.
113
Methane in
Mixture.
7
^ of Second
Limit of
Mixing.
211. 5
58.8
SO. 8
127
136.5
32.5 211
28.4 206
60.2
50.2
125.3
136.8
9-3
12
201.5
198.8
46.6
42.8
141
144
24.5 203
21.6 200
41
30.8
144.2
146
13.7
16.4
199- 5
200.4
37-8
146
19.2 199
20
145.2
19.8
202.1
33.7
30.3
25. 4
146.5
147
146
15.4 198
13.2
8.1
7
137.6
118. 6
crystals
23.5
28.7
34.5
203.7
208
215.2
Solubility of Sulfur in Phenol, Determined by the Synthetic Method.
(Smith, Holmes and Hall, 1905.)
The mixtures of sulfur and phenol were heated until they were homogeneous
and then cooled to the temperature at which clouding appeared.
fof
Houding.
Gms. Sper
100 Gms.
Phenol.
fof
Cbuding.
89.S
9.1
15s
96.S
10.4
157.5
133.5
15.3
160.5
138
19.9
162
148- s
23-6
164.5
Gms. S per
zoo Gms.
Phenol.
26.3
27.1
28.6
29.6
30.7
fof
Oouding.
166
167.5
170
172
175
Gms. Sper
100 Gms.
Phenol.
31.6
32.4
33.5
34.9
36.5
Reciprocal Solubility of Sulfur and Toluene, Determined by the
Synthetic Method.
(Kruyt, 1908-09.)
Wt. % S in
Limiting fof
Homogenei
Mixture.
Lower.
Upper.
SO. 5
167
250
62
179
223
69.6
180
222
73
180
222
Wt. % S in
Lmutingf
of Homogeneity.
Mixture.
75.7
77.9
83.3
90.5
' Lower.
178
174
160
124
Upper.
221
• « •
223
above 250
705
SULFUB
Reciprocal Solubility of Sulfur and Mbta Xylene, Determined
BY THE Synthetic Method.
(Kruyt, 1908-09.)
Wt. % S in
Limiting t'
of Homogeneity.
Wt. % S in
Mixture.
Limiting t'
of Homogeneity.
Miztttie.
Lower.
Upper.
Lower.
Upper.
SO. 9
181
213
39.9
152
none (230)
49. 1
177
228
84.2
none
«
47.7
172. s
none (?)
86.1
164. s
199
44.2
161. s
" (255)
87
159
202.5
40.4
153. s
" (21S)
90
139
none (220)
Fusion-point data for the system sulfur-tellurium are eiven by Pelabon (1909);
Pellini (1909); Chikashige (191 1, 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.
SULFUB DIOXIDE SQi
Solubility in Water.
(SchOnfeld, 1855; SimB, x86z; Roozeboom, X8S4.)
Schfinfdd.
Vob. SO9 (at o"" mnd
y6o mm.) per i Vol.
O
5
10
IS
20
25
30
35
AO
Sat. SOs
+ Aq.
68.86
59.82
Si-3«
43 S^
36.21
30.77
25.82
ai.23
17.01
H40.
79
67
56
47
39
32
27
22
18
79
48
6S
28
37
79
16
49
77
Gms. SOsper
xooGms-fiiO
at total pceaiure
760 mm.
22.83
19-31
16.21
13 54
11.29
9.41
7.81
S-4I
Sims.
SOs per X Gm. H,0.
8
10
14
20
26
30
36
40
46
SO
Gms.
0.168
0.154
0.130
0.104
0087
0078
0.065
0.058
0.050
0.045
Vols.
58-7
53-9
45 -6
36.4
30.5
27 -3
22.8
20.4
17.4
Roosdioom.
SOi Dissolved
per I pt. HjO
t *. at 760 mm.
O
2
4
6
7
8
10
12
0.236
0.218
0.201
0.184
0.176
0.168
0.154
0.142
Sp. Gr. of sat. solution at o* a 1.061; at lo^ 1.055; at 20^ -> 1.024.
The results of Sims are discussed and recalculated by Fulda, 1909.
I gm. H|0 dissolves 0.0909 gm. SOt « 3473 cc. (measured at 25**) at 25^ and
760 mm. pressure. (Walden and Centnersswer, 1903-03.)
FkEEZING-FOINT DATA FOR THE SYSTEM SULFUR DiOXIDE — WATER.
(Baume and Tykodner, X914.)
f of
Freezing.
Mo]8.SOk
per xoo Mob. Solid Phase.
SQi+HiO.
fof
Freesing.
M0I8.SQ,
per 100 Mois.
SQ|+H,0.
Solid Phase.
0
0 loe
7.7
S-I
SObHydxate
—0.2
0.8
8.3
59
ti
—3 Eutec.
" +SQi Hydrate
9.3
7.1
«
—0.2
2.8 SObHydxate
12. 1
II
M
+3-5
3.3
•
•
•
•
:
6.8
55
12.2
95- 1
«
At the temperature +12.1^ and extending over the range of concentration 11
to 95.1 mols. per cent SOt a second phase rich in SOt separates. This crvstal-
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 SOt
hydrate, and the other at the —74* level, to the SOs rich phase. The diagram is
terminated by a very short branch rising from —74^ to the temperature of solidi-
fication of pure SOi (—72.3*).
SULFUB DIOXIDE
706
Solubility of Sulfur Dioxide in Water at Different Pressures.
Results at o''.
in
mm. Hg.
0.4
35
29.4
109.4
Gum. S0»
per 100 cc.
Sat. Sol.
O.OS37
0.237
1.227
3.804
(LindDer, 1912.)
Results at 25*.
Cms. SOb
per 100 oc
Sat. Sol.
0.0534
0.234
I. 212
Results at 50*.
in
mm. Hg.
1-4
"75
87.9
313
3.750
Premire in
mm. Hg.
4.9
30.5
204.5
696
GnM. SOh
per 100 oc
Sat. Sol.
0.0525
0.2276
1. 181
3.628
Solubility of Sulfur Dioxide in Aqueous Salt Solutions.
(Fo«, x9oa.)
Results in terms of the Ostwald Solubility Expression. See p. 227.
Aqueous
Salt Solution.
NH^Cl
NH^r
NH4CNS
NH^O,
NH,NO,
(NH^O,
CdCl,
CdCI,
CdBr,
CdBr,
CdL
Cdl,
CdSO^
CdSO^
KCl
KCl
KBr
KBr
KCNS
KCNS
KI
KI
KNO,
KNO,
NaBr
NaCl
NaCNS
Na^O«
Na^O,
Solubility Coeffident I of S0» in aq. Soludons of ConcentratiGOs:
0.5 Ncnnal
^•=34
^=36
^•=37
4»=33
^=23
fz8=33
^28=31
^6=31
^6=21
^25=33
/„=22
^6=31
^=21
^^34
^=23
^=35
/s6=24
^=25
^=-38
^=26
^=33
^=23
^26=33
^==32
^25 = 35
^•=31
^6=21
xjo N. X.5 N. ajo N. 9.5 X. jjo N.
•S8 36
37
38
.06
39
.76 41.
•25 39
.46
42
.78
46
.06 49.
.78 42
■74
47
.36
52
.26 57.
■96 35
.07
36
.38
37
27 38-
•35 24
•23
24
,78
25
•57 26.
•35 33
.83
34
ZZ
34
•95 35-
•91 23
.14
23
49
23
"93 24.
.66 30
■55
29
.46
38
.16 27.
•73 21
■23
30
■55
30
.02 19.
•91 31
01
30
17
29
.27 28.
.88 31
.46
30
.81
30
60 19.
■27 33 •
76
34 •
16
34 •
74 34.
•75 23 •
06
23-
36
n-
71 23.
.11 39
■71
28.
•24
36
58 25.
•45 20
43
19,
42
18.
31 17-
•42 36
■05
37'
76
39
32 40.
•74 25
15
26.
54
27
94 28.
•94 39
II
42
41
44.
96 48.
•83 27
49
39.
64
31
93 34-
•57 42
38
47
03
51'
81 55-
.63 28
79
32
03
35'
05 38-
.66 44
76
50'
58
56 •
75 62.
•30 30
25
34-
64
38
04 41-
.80 34
■79
35
•77
36
66 37.
•27 24
•03
24
■79
25
.72 26.
•20 33
.61
■
» •
•
• • • •
•76 34
■54
35
27
36
,36 36.
.46 32
•25
31
.96
31
.76 31.
•44 38
•24
40
■78
43
•37 45 •
.96 31
.14
30
•45
29
•51 28.
.88 31
•35
20
.81
20
.21 19.
37
42.78
17
52.25
01
61.46
01
39 14
66
27 -43
47
35 96
23
24.60
09
26.06
23
18.68
15
27.46
70
19.17
98
35-77
99
24.30
14
23.76
41
16.25
96
42.27
93
30.02
87
52.26
12
36.14
87
61.26
13
42.94
63
68.36
87
45-43
57
38.52
54
27 -33
84
• « •
37-74
SI
31-36
86
48.34
66
28.44
75
19.27
The author also ^ves a series of determinations in which a mixture of SOs + COs
is used for saturatms the solutions, thus changing the concentration of the SOs
and yielding results for certain partial pressures of this gas.
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 SOi dissolved in water
and in the aqueous solution. The exact manner in which these calculations were
made is not clearly explained,
707
SULFUB DIOXIDE
Solubility of Sulfur Dioxide in Sulfuric Acid of 1.84 Sp. Gr.
polate<
1 from ongina
1 results.
(Dunn, z88a.)
Sp. Gr.
dfSat.
Coeffident
Sp. Gr.
Coefficient
i*.
of Afaaocp-
t*.
of Sat.
01 Afaaocp-
Solution.
tioa (760 mm.).
Soludon.
tioa (760 mm.)
0
• • •
53 0
50
1 .8186
95
10
I .8232
35 0
60
1. 8165
7.0
20
1 .8225
25.0
70
1. 8140 -
SS
25
1. 8221
21.0
80
I.8112
45
30
1. 8216
18.0
90
1.8080
4.0
40
1.8205
13 0
•
Solubility of Sulfur Dioxide in Aqueous Sulfuric Acid Solutions.
(Dumi; see also Kolb, 187a.)
Sp. Gr. of
Approodmate Coeffident
Sp. Gr. of
AppnoDiiuiti
1 Coefficient
t\
HtSO«
Percent
of
t*.
HsSO«
per cent
of
SoltttioQ.
HaSO«.
AbeorptioQ.
■
Solution.
H1SO4.
Abaorptlor
6.g
I 139
20
48.67
15-2
I 173
25
31-82
6.9
i-3«>
40
45 38
16.8
1.151
31
31-56
S.6
1.482
58
39-91
14.8
1.277
36
30.41
9.8
I 703
78
29.03
151
1.458
S6
29.87
5-5
1.067
10
36.78
15 -6
1.609
70
25-17
6.0
I .102
15
3.408
15-0
1-739
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, 189a; Schuke, z88x.)
In Ethyl Alcohol
at 760 mm.
^•^ Gms. SOa per xoo Gm«.
Solution. CiH«OHt
O 53 5 "5-0
7 45 .0 81 .0
12.3 39.9 66.4
18.2 32.8 48.8 (17
26.0 244 32.3
In Methyl Alcohol
at 760 mm«
Gms. SO9 per xoo Gms.
Solution.
71. 1
59-9
52.2
.8^)44.0
31-7
CHiOH.
246.0
149-4
109.2
78.6
46.4
In Several Solvents
at o"* and 725 mm. (S.)
SOa per x Gm .Solvent
SJvent.
Grams. Vols.
Camphor o . 880 308
CHjCOOH 0.961 318
HCOOH 0.821 351
(CH,)jCO 2.07 589
SOjClj 0.323 189
Solubility of Sulfur Dioxide in Chloroform.
(Lindner, X9xa.)
Results at o^ Results at 25*.
Pleasure in
Gms. SO^
Pressure in
Gms.S0b
mm. Hg.
per xoo cc
Sat. Sol.
per xoocc
Sat. Sol.
2.7
0.0701
5.7
0.0669
5.6
0.1790
12.9
O.1712
22
0.6982
48
0.6728
90.2
3-097
200.2
2.954
219.6
8.217
488.8
7-^39
SULFUB DIOXIDE
708
Solubility of Sulfur Dioxide in Several Solvents.
(Lloyd, 19x8.)
The dry, air free, SOi 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.
Cms. SQ
1 per Liter of Saturated Solution in:
f.
Benzene.
Nitio-
beoxcDC.
Toluene.
cNHra-
tohicoe.
Acetic
Anhydride.
- s
• « •
• • •
196
0
• • •
* • •
148(^-1.23
+ 5
• • •
• • •
136
10
• • •
• • .
122
IS
3"-4
290.8
114
20
267.4
217s
236
106
25
227.9
170.4
192.2
99
30
127. s
190
124.4
160.7
90
40
82.9
132
93-6
118. s
• • .
SO
60.3
98.7
77.2
87.2
• ■ .
60
34
78.6
S4.7
68.8
• ■ .
Distribution of Sulphur Dioxide at 20° between:
(McCrae and Wilaon, 1903.)
Water and Chlorofonm.
Gitts. SOs per
Liter in:
Aq.
Layer.
1-738
1-753
2.346
2.628
3 058
3-735
4.226
5.269
6.588
31.92
33-26
CHCIf
Layer.
1. 123
1 .122
1-703
1.897
2.385
3.062
3.626
4.798
6.183
33 84
37-25
Gm. E<^uiT. iiSOt
per Liter in:
Aq.
Layer.
00543
0.0547
0.0732
0.0821
00955
O.I166
O.I319
o . 1645
0.2057
0.9968
1.038
CHCls
Layer.
00351
0.0350
0.0532
0.0592
0.0745
0.0956
O.II32
o . 1498
0.1930
1.056
1. 163
Cone.
of
HQ.
0.05
it
it
ti
O.IO
<(
It
a
0.2
((
<<
«
0.4
Aq. HCl and Chloroform.
EquiT. i:
r Liter in:
Cms. SO3 per
Liter in:
Gm.
per
4SQ»
Aq.
Layer.
1.86
3-07
4.28
5-34
1-25
2.78
3.86
5. 161
1.268
1. 914
2.464
3-967
1 .202
1.894
CHCli
Layer.
Aq.
Layer.
1.46
0 0581
2.83
0.0960
4.07
0 . 1336
5 42
0 . 1667
1. 41
0.039
3-08
0.0868
4.08
01199
572
O.1612
I-5I
0.0396
2.27
0.0597
3 04
0.0769
4.90
0.1239
Z.61
0.038
2.26
0.059
CHOa
Layer.
0.0456
0.0884
O.I271
0.1692
0.044
0.0962
0.1275
0.1784
0.0471
O.07I0
00949
0.1530
0.0504
o .0706
Freezing-point data for mixtures of sulfur dioxide and sulfuryl chloride (SQiCh)
are given by van der Goot (1913).
SULTUBIC ACID H,S04 (Sulfur Trioxide, SO.).
Solubility in Water.
(Landoldt and BOmstein, "Tabellen," 4th Ed., pp. 472-3* xgu.)
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 SOt. The complete results are given on the following page.
709
SULFURIC ACID
SOLUBILITT OF SULFURIC ACID IN WaTBR, DbTBRMINED BY THE
Freezing-point Method.
Gms.
Gms.
H,S04
Gms. SOi'
H,S04
Gms. SO^
f.
per 100
per 100 Gms. Solid Phase.
f.
per 100
per zoo Gms.
SoUd Phase.
Gms.
Sat. Sol.
Gms.
Sat. SoL
Sat.SoL
Sat. SoL
lO
16.25
I3.2S(I)(5) I«
— 10
77.75
63.5 (3)
S0b.2Hfl0
20
24
I9.5(0(2)(3) "
0
80.25
65.5 (2)
i<
30
28.5
23.25 (2)
+ 8.35'
•84.5
68.98 (2)
u
40
31-25
^5-S 2) "
8.81
84.S
68.98 (l)
u
so
33-5
27.25 (i) (2) "
0
88.25
72 (2)
u
60
35.25
28.75 (i)
— 20
91.5
74.75 (l)
((
70
36.7s
30 (2)
-30
92.5
75.5 (l)
«f
75
38
31 (2) " +SQ,.sH^
-38
93
76 (2)
"+S0^H/)
70
39
31.75(2) SOi-sHiO
-30
93.75
76.5 (4)
SQ|.Hfl0
60
41-5
33.75(2) "
— 20
95.25
77.75 (4)
<i
SO
44
36 (2) "
— 10
96.25
78.5 (i)(4)
II
40
47-75
39 (2) "
0
97-75
79.75 (4)
fi
3<^-.
53.25
43.25(2) "
+10
99.75
81 (4)
11
25*
57.65
47.06 (2) "
10-35
100
81.62 (i)(3)(7)(4)
30
61
49.75(2) "
10
• « •
82 (4)
II
40
65.25
53-25(2) "
0
• ■ •
83.25 (4)
II
60
70.7s
57-75 (3) " (unstable)
— 10
• • •
84.5 (4)
II
70
73-25
5975(3) " " +SQ|.»H^
— 12
• • •
85 (4)
" +S0,.iH|Q
60
73.50
60 (3) SO».aH^ CunsUble)
— 10
• • «
85-25 (4)
86 (4)
SQ|.»H^
SO
74.25
60.5 (3)
0
• • •
li
SO
68
55-5 (2) SO,.sIV)+SQ|.3H^+io
• ■ •
86.75 (4)
i«
45
68.5
56 (6) SO,.3H4b
20
• • •
87-5 (4)
u
40
71
58 (6) "
30
• • •
88.5 (4)
l«
38.9'
* 73.14
59.69.(6) «
36^
• • «
89-89 (4)
II
40
74.25
60.5 (6) "
30
• • •
90.5 (4)
II
41
74.75
61 (6) " +SO,.iHiO
20
• • •
91.5 (4)
<l
40
74.75
61 (4) SQ|.3H,0
zo
• • •
92.25 (4)
93 (4)
l(
30
75.25
61.S (4)
6.5
• • •
" +<?)
20
76.5
62.5 (3)
• m
.pt.
(I) ■
-Pfaundler and Schnetw (187s); (a) -Pickt
ving (z89<
>);(3) -'
•
Thilo (iSoa); Pictet (1894); (4)
" Knietsch (1901); (5) " RttdorfF (1863); (6) >
(1890-91); Lespieau (1894) and Giran (i9i3).
Biron (1899); (7) ■- Marignac (1853). See also Pickering
Solubility of Sulfuric Acid in Benzene Solutions of Valeric
Acid at 18**.
(Gurwitsch, z0z4.)
The mixtures were shaken with excess of 95.8% HsS04 at o® and then brought
to equilibrium at i8^
Gms. Valeric
Add per zoo
Gms. Valeric
Add+Benzene.
Gms. HsS04
per 100 Gms.
of the
Sat. Solution.
0= Pure benzene
0
0.584
1.62
3 64
7.60
0.052
0.104
0.226
0.378
17s
0.454
TANNIC ACID 710
TANNIC ACID
When a sample of tannic acid of apparently veiy 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 eviclent 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 ^o to 400 gms. acid per 100 gms. of alcohol. (Seidell, 1910.)
100 gms. glycerol dissolve 48.8 gms. tannin at 15-16^. (Osaendowaki, 1907.)
100 gms. trichlorethylene dissolve 0.012 gm. tannin at 15^. (Wester and Bniins, 1914.)
TANTALUM Potassium FLITORIDB TaKsF,.
Solubility in Aqueous Hydrofluoric and Potassium Fluoride Solutions.
(Ruff and Schiller, 19x1.)
The tantalum salt was purified by repeated crystallizations from pure anhydrous
HFl. After drying at 120°, it was shaken in platinum flasks for 3 tiour periods at
constant temperature with HFl or KFl solutions or both together. The saturated
solutions were filtered by means of a platinum funnel and subjected to analysis.
Mixture Shaken
f.
Gms. per
100 Gtns. :
Sat. Sol.
SoUd Phaae.
in Pt. Flask.
TaH«.
KF.
HF.
K,TaF,+H,0
18
0.25
0.12
0.029
K.Ta/?.F«+K,TaF
" +aq.4.77%KF
18
O.IO
4-79
0.074
M
" +aq. 7.35% KF
16
0.09 •
6.73
0.015
f<
" +aq.4.47%HF
18
1-33
0.56
4.47
K.TaF»
" +aq. 4.2 %HF
18.5
1.24
0.52
4-2
II
" +aq. 24.3 %HF
18
535
2.25
24.3
u
" +aq. 10.44% HF+ )
21.92% KF S
18
0.036
21.93
10.44
M
" +H,0
85
2.18
1.69
0.85
K.Ta^J«+K,T«F,
" +aq. 4.77% KF
85
0.96
S.27
I. 17
<t
" +aq.4.47%HF
90
573
2.41
4.47
K,TaF,
" +aq. 4.2% HF
90
6
2.52
4-2
II
" +aq. 23.3%HF
90
10.9
4. 59
24.3
i<
" +aq. 21.92% KF+ )
10.44% HF S
90
1. 18
22.42
10.44
u
The solid phases were identified only by th^ir crystal forms and it is possible
that still others may be present.
TABTABIC ACIDS 'C,H2(0H)s(C00H)f. d, I, Bind racemic
Solubility of Each Separately in Water.
(Leidie,i883.)
t*. Grams Tartaric Add per xooOms.'HzO. t°. Gms. Tartaric Add per xoo Gms. HsO.
r-
Dextro
Racemic
Racemic
Dextro
Racemic
Racemic
and Laevo
Ac.
Ac.
and Laevo
Ac.
Ac.
Adds.
Anhydrous.
Hydrated.
Adds.
Anhydrous.
Hydrated
0
115.04
8.16
9 23
SO
195.0
50.0
59 54
10
125.72
12.32
14.00
60
217-55
64.52
78-33
20
139 -44
18.0
20.60
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
152-74
40
176.0
37 0
43 32
100
343-35
137.80
184.91
100 gms. HsO dissolve 140.8 gms. tartaric acid at 15^ The Sp. Gr. of the sat.
solution is 1.31, (Greenish and Smith, xgosj
711
TABTABIC ACID
SOLUBILITT OF TARTARIC AciD IN ALCOHOLS.
(Timofeiew, 1894.)
Alcohol.
f.
per 100 Gms.
Solvent.
r
Alcohol.
f.
per TOO Gms.
Solvent.
Methyl Alcohol
- 3
67. S
Ethyl Alcohol
+23
28.9
((
+19.2
70.1
((
39
31.8
i<
23
73.2
Propyl Alcohol
- 3
8.74
«
39
77.3
«
+19.
2 10.85
Ethyl Alcohol
- 3
22.4
n
23
11.85
((
+192
27.6
«i
39
14.4
Solubility of Tartaric Acid in Aqueous Ethyl Alcohol Solutions at 25**.
(Seidell, 1910.)
Wt. Per cent
dmoH
in Solvent.
O
10
20
30
40
50
Sat. Sol.
1. 321
1.300
1.276
I. 251
1.220
1. 184
Gms. CaHt(0H)t(C00H),
per zoo Cms.
Sat. Sol.
57-9
56
54.1
52
49.6
47
Solvent.
137-5
127.3
117. 9
108.3
98.4
88.6
Wt. Per cent j ^j
in'^^eni. Sat. Sol.
60
70
80
90
95
100
1. 142
1.095
1.040
0.973
0.937
0.905
Gms. C|H|(0H),(C00H)s
per zoo Gms.
Sat. Sol.
43-9
40.2
35-3
29
25.4
21.6
Solvent.
78.3
66.9
54.6
40.8
34.1
27.6
Solubility of Tartaric Acid in Several Solvents.
Solvent.
Sp. Gr. of
)lvent.
i>p.
So\
Amyl Alcohol dn = 0.817
Benzene dn — 0.873
Carbon Tetrachloride (^25 = 1.587
Ether ^11 = 0.711
<(
Dichlorethylene
Trichlorethylene
du of
Sat. Sol.
0.824
0.875
1.589
0.715
f.
25
25
25
25
15
15
15
Gms. aHs(0H)r
(COOH)i per zoo
Gms. Solvent.
Authority.
(Seidell, x^xo.)
3.50
0.0086
0.0189
0.61
0.40 (Bouigoin, 1878.)
0 . 005 (Wester & Bruins, '14.)
0.005
<(
<t
If
Distribution of Tartaric Acid between Water and Ether.
Results at I5^
Gms. Mds. per Liter.
(Pinno^i 19x5.)
Results at 27^
H«0 Layer, c.
1.402
0.790
0.446
Ether Layer, c'.
0.0072
0.0037
0.0022
c_
Gms. Mob. per Liter.
, * ,
HtO Layer, c. Ether Layer, c'.
197
216
210
1.625
0.857
0.427
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 i forms of the diformalic (jerivative 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 « dimethyl ester of tar-
taric acid are given by Centnerszwer (1899).
PyroTABTABIG ACID (Methyl Succinic Acid) CH,.CH(COOH).CH,(COOH).
100 gms. H|0 dissolve 51 gms. CHtCH(C00H).CH2C00H at iqlj*.
(Timofeiew, 1894.)
PyroTABTABZC ACID
713
Solubility in Alcohols.
(Timofdew, 1894.)
AloohoL
r.
Gms. Add
per 100 Cms.
Solvent.
AloohoL
r.
Oiiis.Acid
per zoo Gm.
Solvent.
Methyl Alcohol
-18. s
S3
Ethyl Alcohol
19s
72.4
tc
+19
109.8
Propyl Alcohol
19
44.9
u
+195
112.5
tt
19s
471
Ethyl Alcohol
+19
70.8
100 gms. 95% formic add dissolve 17.8 gms. pyrotartaric acid at 18.5^
(Aachan, 1913.)
TEBPIN HTD&4TE C,oHu(OH),.HA
100 cc. H/) dissolve 0.36 gm. terpin hydrate at 15-^0^
100 cc. 90% alcohol dissolve 7.1 gms. terpin hydrate at 15-^0^.
(Squire and Gaines, 1905.)
TBLLUBIUM Te.
100 gms. methylene iodide, CHiIi, dissolve o.i gm. Te at I2^ (ReCgeis, 1893.)
Distribution of TELLUkiuii between Aqueous Hydrochloric Acid and
Ether at Room Temperature.
(Biyiius, 19x1.)
When I gm. of tellurium as the chloridei TeCU, is dissolved in 100 cc. of aqueous
HCl and shaken with 100 cc. of ether, the following per cents of the metal enter
the ethereal layers. With 20% HCl, 34 per cent; 15% HCl, 12 per cent; 10%
HCl, 3 per cent; 5% HCl, 0.2 per cent and with 1% HCl, 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).
TBLLUBIC ACID HtTeO«.2H,0.
Solubility
IN Water.
(Biyiius, X90Z.)
Gms. Mob.
Gms.
H|Te0«per
100 (jms.
Mols.
^ H|TeO« per BtTtOi per
* * xoo Gms. xoo Mols.
Solid Phase.
f.
HfTeOiper
100 Mols.
SoUd Phase.
SoL H|0.
Sol.
H|0.
0 13.92 1.51
HKTeO«.6H|0
30
33 36
4.67
H|Te04.aH^
S 17.84 2.03
i«
40
36.38
S-33
M
10 26.21 3.31
(1
60
43 67
7.04
M
IS 3279 4SS
i<
80
Si-SS
9-93
II
10 25.29 3.15
H|TeO«.9H^
100
60.84
14.52
II
18 28.90 3.82
(1
no
67
19
11
TBLLUBIUM DOUBLE SALTS
Solubility of Tellurium Double Bromides and Chlorides in Aqueous
Hydrochloric and Hydrobromic Acids at 22®.
(Wheeler, 1893a.)
Tdlttrium Double Salt.
Te Caesium Bromide
Te Potassium Bromide
Te Rubidium Bromide
Te Caesium Chloride
Te Rubidium Chloride
Formula.
Solvent.
Gms. Double Salt per xoo
Gms. Solvem
TeBr4.2CsBr Aq. HBr
TeBr4.2KBr
TeBr4.2RbBr
TeCl4.2CsCl Aq. HCl*
TeCl4.2RbCl
it
of z .40 Sp. Gr.
ofx^Sp.Gr^
0.02
0.13
6.57
62.90
0.25
3.88
0.05
0.78
034
13 09
* sp. Gr. of Aq. HG solutioDS i.a and z.05 respectively.
71.^
TELLURIUM IODIDE
TELLUBIX7M TetralODIDE Teh.
Solubility in Mixtures of Aqueous Hydriodic Acid and Iodine at 25®.
(Meoke, 191 2.)
*
Weighed amounts of Teh + I + 6j wt. % HI solution were shaken in sealed
glass tubes for 10 days. Both the clear saturated solution and the solid phase
were analyzed.
\
Composition of Original Biixture
in Gms.
Gms. per 100 Gms.
Solutiouf
Solid Phase.
Tcl».
3
2
2
3
Excess
I.
1-5
0.5
0.5
3
None
64% HI.
19-25
9.61
9.61
8.09
Tel,.
12
13
13s
20
9
I. '
II. 7
0
8.2
21.8
0.19
Small amt. TeI,.HI.8H^
nuch
small amt. *'
TeI«.HI.8H^
2
4
3
None
9
10
7
Excess
9.10
9.27
9.03
5 (cc-)
10
IS
17-5
None
52.4
47.7
47.9
61. 1
Iodine
M
«
M
THALLIUM ALUMS
Solubility in Water at 25*.
(Locke, 190Z.)
Salt per zoo Grams HfO.
Alum.
Formula.
Tl Aluminum Alum
Tl Vanadium Alum
Tl Chromium Alum
Tl Iron Alum
See also pp. 31 and 32.
TIAl(S04),.i2H20
TlV(S04),.i2HjO
TlCr(S04)2.i2H20
TlFe(S04)a.i2H30
Gms.
Gms.
Gm.
Anhydrous.
Hydrated.
Mob.
75
II .78
0.0177
25.6
43 31
00573
10 48
16.38
0.0212
36 IS
64.6
0.0799
THALLIUM BROBCATE TlBrOt.
One liter saturated aqueous solution contains 3.463 gms. TlBrOt at 19.9^ (BOtt-
ger, 1903) and 7.355 gms. at 3975*- (Noyes and Abbot, 1895.)
THALUUM BROBODE TlBr.
One liter sat. aqueous solution contains 0.238 gm. TlBr at 0.13*^, 0.289 S™* &t
9.37*^, 0.4233 gm. at 18^ and 0.579 gm. at 25.68^ (Kohlnusch, 1908.)
Solubility of Thallium BROMroE in Aqueous Solutions op Thallium
Nitrate at 68.5®.
(Noyes, 2890.)
Gms. Mob. per Liter. Gms. per Liter.
TINO,.
0
0.0163
0.0294
0.0955
TlBr.
0.00869
0.00410
0.00289
0.00148
TINO,.
0
4.336
7.820
25.400
TlBr.
2.469
1. 164
0.821
0.420
F.-pt. data for mixtures of TlBr + TlCl, TlBr + Til and TlCl + Til are given
by Nlonkemeyer (1906). Results for TlCl + SnCli and TlCl + ZnCli are given
by Korreng (1914).
THALLIUM. CARBONATE TI,COt.
Solubility in Water.
(Crookes, 1864; Lamy, X863.)
t*. 15.5*. i8*. 6a*. xoo*. 100.8*.
Gms. TI2CO8 per 100 gm^ HsO 4.2(0.) 5.23 12.85 27.2(0.) 22.4
^e
THALLIUM CHLORATE 714
THALLIUM CHLORATE TlClOt.
SOLUBILITT IN WaTBK.
(Muir, 1876.)
t*. o*. lo*. so*. 8o*. 100"
Gms. TlClOs per 100 gms. H^O 2 3.92 12.67 36.65 57.31
One liter sat. aq . solution contains 38.5 1 gms. TlCld at 20*. (Noyes and Farrd, 191 1.)
One liter of aqueous solution, saturated with both salts, contains 30.4 gms.
TlClOi + 34.43 gms. TI1SO4 at 20''. (Noyes and Fand, igxx.)
Solubility of Mixbd Crystals of Thallium Chlorate and Potassium
Chlorate in Water at 10^.
(Rooxeboom, 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.
Mols. percent
KQQi mMixed
Cxystala.
O
2
12.61
25.01
36.30-97.93
99.28
99.60
99.62
99.67
100
Solubility of Mixed Crystals of Thallium Chlorate and Potassium
Chlorate in Water at Different Temperatures.
(Quoted by Rabe, 1902.)
100 gms. H«0 dissolve 2.8 gms. TlClOi + 3.3 gms. KClOi at o^.
^* HjO dissolve 10 gms. TICIO, + 1.5 gms. KClOi at 15*.
H:K) dissolve 12.67 gms- TlClOi + 16.2 gms. KClOi at 50*.
HiO dissolve 57.3 gms. TlClOj + 48.2 gms. KClOj at 100**.
THALLIXTM PerCHLORATE TICIO4.
Solubility in Water.
(Carbon, 19x0.)
« ^, Gms. Tia04 e„ /^ Gms. TlOQi per
o 1.060 6 50 1.251 39.62
ID 1.07s 8.04 70 1.430 65.32
30 I. 146 19-72 80 1.520 81.49
100 gms. HtO dissolve 10 gms. TICIO4 at 15^ and 166.6 gms. at 100*.
(Roscoe, 1866.)
Gmfl. per
1000 cc.
Mg. Mob.
per 1000 cc.
Sp.Gf.
Solution.
Solution.
^
'xiao^
KQOt.
TICICV
KQO,. '
Solutions.
25-637
• ■ •
89.14
• • •
I. 0210
19.637
6.884
68.27
56-15
1.0222
12.001
26.100
41.73
212.89
1.0278
9-036
40.064
31-42
326.79
I .0338
7.885
46.497
27.42
379.26
I -0359
7-935
46.53s
27.60
379-57
1.0360
6.706
46.410
23.32
378.5s
1.0357
6.723
47.109
23-37
384-25
1.0363
4.858
47-3"
16.89
385-91
1.0345
2.769
47 • 134
9-63
384.46
1-0330
• • ■
49-925
• • ■
407.22
1-0330
715
THALLIUM CHLOBmS
THALLIUM CHLORIDE TlCl.
Solubility in Water.
(Average cnrve from results of Npyo. 1893; Bdtt^er, 1903; Kohliauflch, 1904; Hebberling; Crookes;
Lamy. The results oTBerkeley, 1904 are also given.)
r.
Gms. na per Liter.
r.
Gms. TIQ per Liter.
0
2.1 (av.) 1.7 (B.)
25
3.86 4
10
2.5' 2.4
30
4.2 4.6
20
3.3 3.4
40
5.2 6
50
6.3 8
t*. Gms. TlCl per Liter.
60 8 10.2
80 12 16
100 18 24.1 (99.3°)
The results of Berkeley are in terms of gms. of TlCl iter 1000 gms. HtO but
since the densities of the solutions are approximately i in all cases, except for
temperatures above 60®, the differences are n^ligible. The Sp. Gr. of the sat.
sol. at 9^.3® is 0.9787 and the figure 24.1, there&re, becomes 23.58 gms. per liter.
One liter sat. solution in water contains 2.27 gms. TlCl at 9.54^, 3.05 gms. at
17.7^ and 3.97 gms. at 25.76^ (Kohlnuscfa, 1908.)
Solubility of Thallium Chloride at 25^ in Aqueous Solutions of:
Acetic Acid.
(Hill. 1917.)
rormaHtyof TIQ per Liter.
.UUtUUUll. Gms. Gm. Equiv.
0 3.8515 0.016085
0.0501 3.8375 0.016027
0.0958 3.8326 0.016006
0.263 3.7503 0.015662
0.524 3.6539 0.015258
Normality <rf
Aq.HNOb.
0
0.4977
1.0046
2.0452
4.0170
Nitric J
(Hill and Simi
dt$ of
Sat. Sol.
0.996
I. 0184
1.0359
1.0705
I . 1362
Acid.
QODs, 1909.)
TlCI per Liter.
' Gms. Gm. Equiv.
3.951 0.0165
5.937 2.475
6.882 2.875
8.143 3.401
9.925 4.145
Solubility of Thallium Chloride in Aqueous Solutions of Salts
with a Common Ion at 25®.
(Noyes, 1893.)
Aqueous
Solution of:
Gms. Equiv.
Added Salt
per Liter.
Gms. Equiv.
Dissolved TlCl
per Liter.
•
Aqueous
Solution of:
GmsL Equiv.
Added Salt
per Liter.
(3ms. Equiv.
Dissolved Tia
per liter.
Water alone
0
O.OI612
Mga,
0.025
0.00904
NH4CI
0.025
0.00877
«
0.050
0.00618
«
0.05
0.00593
It
O.IO
0.00413
II
0.20
0.00271
It
0.20
0.00275
BaCla
0.05
0.00620
MnQs
0.025
0.00898
((
O.IO
0.00425
«
0.05
0.00617
CdCli
0.025
0.01040
<(
O.IO
O.OQ412
((
0.05
0.00780
((
0.20
0.00286
«
0.10
0.00578
KCl
0.025
0.00872
n
0.20
0.00427
II
0.05
0.00593
CaCls
0.025
0.00899
tt
O.IO
0.00399
((
0.05
0.00624
tt
0.20
0.00265
tt
O.IO
O.OQ417
It
0.80
0.00170
(i
0.20
0.00284
NaCl
0.025
0.00869
CuCLt
0.025
0.00905
({
0.05
0.00592
tt
0.05
0.00614
It
O.IO
0.00395
ti
O.IO
0.00422
II
0.20
0.00271
tt
0.20
0.00291
TlClQi
0.025
0.00897
Ha
0.025
0.00869
It
0.025
0.00894
tt
0.05
0.00585
TTNQi
0.025
0.00883
tt
O.IO
0.00384
It
0.05
0.00626
tt
0.20
0.00254
tt
O.IO
0.00423
THALUIIM CHLOBIDI
716
Sqlubiuty of Thallium Chloride in Aqueous Salt Solutions at 25^
(Noyes» 1890; Nqyes and Abbott, 1895; Geffckai, 1904.)
Aq. Sdt Solatioii.
Ammonium Nitrate NHiNOb
f(
tt
«
Barium Chloride BaCh
tt
Cadmium Sulfate CdSOi
It
tt
Hydrochloric Add HD
tt
tt
Lithium Nitrate LiNOb
Potassium Chlorate KGOb
Potassium Nitrate KNOb
tt
tt
tt
tt
tt
tt
Sodium Acetate CHiCOONa
tt
tt
tt
Sodium Nitrate NaNUi
tt
tt
tt
tt
Sodium Chlorate NaCl(^
tt
tt
tt
tt
ThalliumBromateTlBiOi (at 39.75")
Thallium Nitrate TlNQi
tt
tt
Thallium Sulfate TUSOi
tt
Thallium Thiocyanate TISCN
(at39.7S">
tt
G.Mob.
. per Liter.
Gms. p<
'SaU. "
er Liter.
Salt.
Tia
Tia.
0
O.O1612
0
3.861 (G.)
OS
0.02587
40.02
6.209
z
O.03121
80.05
7.473
3
0.03966
x6o.io
9-497
0.0283
0.00857
S.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. 4X
6.081
0. 1574
0.0309
32.82
7.399
0.0283
0.00836
X.032
2.002 (N.)
0.0560
0.00565
2.043
1.353
0. 1468
0.003x6
5.357
0.757
o.S
0.02542
34.53
6.085 (G.)
I
0.03035
69.07
7.266
3
0.03785
X38.14
9063
3
0.04438
207.21
10.630
o.S
0.0237
6X.28
5.674 (G.)
0.015
0.0170
1. 517
4.070 (N.)
0.030
0.0x79
3033
4.386
0.0787
0.0192
7. 775
4.597
0. 1574
0.0212
15.920
5.076
o.S
0.0257
50.55
6.153 (G.)
I
0.0308
XOI.IX
7.375
3
0.0390
202.22
9340
0.015
0.0x68
1. 231
4.023 (N.)
0.030
0.0172
2.462
4. 118
0.0787
0.0185
6.46
4.430
O.IS74
0.0196
12.92
4.693
o.S
0.02564
42.50
6.i39(G.)
I
0.03054
85.01
7.313
3
0.03851
170.02
9.22Z
3
0.04544
255.03
X0.88
4
0.05128
340.12
12.28
o.S
0.02320
53.25
5.555 (G.)
X
0.02687
106.5
6.433
3
0.03060
213
7.326
3
0.03303
319.5
7.909
4
0.03850
426
9.215
0.01567
0.01959
5.20X
4.690 (N.ftAO
0.0283
0.0083
7.518
1.987 (N.)
0.0560
0.00571
14.89
1.368
0.X468
0.00332
39.05
0.795
0.0283
0.00886
14.27
2. 121 (NO
0.0560
0.00624
28.23
1.494
0.0107
0.0119
2.802
2.849 (N.)
0.02149
0.01807
5.632
4.326(N.ftA0
Note. — In the case of (he results for thallium bromate and thallium thio-
cyanate at 39.75^, the solut£ons were saturated with respect to these salts as well
as with respect to thallium chloride.
717
THALLIUM CHLORIDE
Solubility of Thallium Chloride in Aqueous Solutions of Salts at 2<^*
(Bray and Winninghoff, 19x1.)
Solvent.
Satuxated Solution.
Salt
Present.
Gms. Equiv.
Salt, per Liter.
s
dmm of'Aq.
^Ivent.
Gms. Equiv.
Salt per Liter.
i.. of Sat.
Sol.
Gms. Equiv.
TIG per Liter.
None
• • •
• > •
...
0.9994
0.01607
KNQi
0.02001
0.9973
0.020
1.0009
O.OI716
(1
0.05000
0.9992
0.04997
1.0028
0.01826
u
0.10005
1.0023
0.09998
1.0063
O.OI961
it
0.3002
I. 0145
0.3000
I. 0194
0.02313
CI
1.0005
1.0568
0.9996
1.0632
0.03072
KtS04
0.01997
0.997s
0.01996 .
I. 0012
0.01779
u
0.05000
0.999s
0.04996
1.0037
0.01942
it
O.IOOO
1.0030
0.09989
1.0074
0.02137
u
0.3000
I. 0167
0.29966
I. 0221
0.02600
«
I
1.0628
0.9986
1.0698
0.03416
TljSOi
0.0200
1.0007
0.01999
1.0028
0.01034
i<
0.0500
1.0076
0.04999
1.0090
0.006772
it
O.IOOO
I.OI91
0.09997
1.0200
0.004679
One liter of water dissolves 2.7 gms. thallo thallic chloride 3TICI.TICU at I5''~I7^
and 35 gms. at 100^. (Crookes, 1864; Lamy; Hebbeiling.)
THALLIUM CHBOBCATE Tl,Cr04.
100 gms. H|0 dissolve 0.03 gm. TlsCrOi at 60^, and 0.2 gm. at 100^.
(Browningand Hutchnifl, 1900.)
One liter of aq. 31 per cent KOH solution dissolves 18 gms. TlsCrOi.
(Lepierre and Ladiand, 1891.)
One liter of H/) dissolves 0.35 gm. thallium trichromate, TliCriOio, at 15^,
and 2.27 gms. at 100^. (Ciookes, 1864.)
THALLIUM CTANIDB TICN and Double Cyanides.
Solubility in Water.
(Fronmttller. 1878.)
Cyanide. Formula. Gms. Salt per 100 Gms. H^.
Tl Cyanide TICN 16.8 at 28.5^
Tl Cobalti Cyanide TUCo(CN)e 3.6 at o**; 5.86 at 9.5**; 10.04 at I9.5^
Tl Zinc Cyanide 2TlCN.Zn(CN)2 8.7 at o**; 15.2 at 14**; 29.6 at 31**.
Tl Ferro Cyanide Tl4Fe(CN)«.2HiO 0.37 at 18'*; 3.93 at 101°. (Lamy.)
THALLIUM FLUORIDS TIF.
100 gms. H/) dissolve 80 gms. TIF at 15*
(BOdmer, 1865.)
THALLIUM HTDBOXIDB TIOH.
Solubility in Watbk.
(Bahr, 191 1.)
r.
dxpOt
Sat. SoL
Mols. TIOH
Gms. TIOH
f.
Mob. nOH
Gmt.T10H
per Liter.
per Liter.
per Liter.
per Liter.
0
I. 231
1. 151
254.4
44.5
2.442
539.8
18.5
1. 317
1.554
343.4
54.1
2.940
649.7
29
1.342
1.803
398.5
64.6
3.601
795.8
32.1
1.377
1. 861
411. 2
78.5
4.673
1033
36
1. 417
2.075
458.6
90
5. 705
1 261
40
1.446
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 lODATE 718
THALLIUM lODATE T1I0».
One liter aq. solution contains 0.^78 gm. TllOt at 20^ (Btttner. 1903.)
One liter aqueous solution contains i.76.ior^ mols. TllOt at 25^ » 0.667 8^-*
determined by means of electrodes of the third kind. (Spencer, 19134
THALLIUM lODIDB Til
One liter sat. solution in water contains 0.0362 gm. at 9.9^ 0.056 gm. at 18. i*
and 0.0847 gm. at 26®. (KoUnuich, 1908.)
Solubility op Thallium Iodidb in Water.
(Avenge icsults from Bflttger, 1903; Kohlrauich, 1904-05; Werther; Crookes, 1864; Lamy; Hebberling.)
r. ©•. lo*. 40*. 6o*. 8o*. loo*.
Gms. 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. TlCl.
One liter of 6) per cent aq. ammonia dissolves 0.758 gm. TlCl.
One liter of 90 per cent alcohol dissolves 0.0038 gm. TlCl.
One liter of 50 per cent alcohol dissolves 0.027 gm. TlCl. (Long. 1888.)
Data for the temperatures of solidification of mixtures of Til and TlNOi are
given by Van £yk (1901).
THALLIUM NITBATE TINO..
Solubility in Water.
(Berkeley, 1904; tee also EUrd, 1894; Crookes; Lamy.)
Gma. TlNOs per 100 Gms. Gms. TlNO> per 100 Gms.
« . *—
Soludon.
Water.
0
3 76
3-91
10
S-86
6.22
to
8.72
9 -55
30
12.51
14-3
40
17-33
20.9
so
23-33
30 -4
» .
Soludon.
Water.
60
31
■55
46.2
70
41
.01
69.5
80
52
.6
III.O
90
66.66
200.0
100
80
•54
414.0
los
85
-59
594 0
Solid phase. TlNOi rhombic.
100 gms. HsO dissolve 43.5 gms. TlNOi + 104.2 gms. KNOt at 58^ (Babe, 1909.)
THALLIUM OXALATE TlsCs04
One liter of saturated aqueous solution contains 15.77 gms. TlsC|04 at 20^ and
18.69 gms. at 25^. (BOttcer, 1903; Abegg and Spencer. 1905.)
SOLUBIUTY OF THALLIUM OXALATB AT 25* IN AQ.. SOLUTIONS OF:
Thallium Nitrate.
Potassium Oxalate.
(Abegg and Spencer.)
(Abegg and Spenoer.)
er Uter.
TljCjO*.
Mol. Con
KsCtO*.
oentratioo. Grama per Liter.
TlNOa. TlsCjO*. TlNOt.
TlsCfO*. 'KaCiO«. TlsCiO«.
CO 0.03768 0.00
18.69
00498
0.0351 8.281 17.42
O.04114 0.0264 . 10.95
13.10
0.0996
0.03565 16.57 17.69
0.0799 0.0195 21.26
9.68
0.2467
0.0390 41 .Q2 19.36
0.1597 0.01235 42.51
6.128
0.4886
0.04506 81.25 22.37
0.9785
0.05536 162.6 27.48
THALLIUM PHOSPHATE (ortho) TUPO4.
One liter of sat. aqueous solution contains 4.97 gms. TUPO4 at 15^ and 6.71
gms. at loo^ (OcMkea, 1864.)
719 THALLIUM PICRATE
THALLIUM PICRATE T10C«Ht(N0t)..
Solubility in Water.
(Rabe, 190X.)
tSins. ' Gntt.
«•• ^52^ G^' Solid PhMC r. ™S<^^- SoKdPhMC
HdO. Hfi.
O 0.135 MooocfiaicRed 45 Z.04 TcicUiiic Yellow
18 0.36 « 47 1. 10 "
30 0.57s " 50 1.205
40 0.825 - 60 1.73 «
47 1. 14 " 70 2.43 ••
~ 100 gms. H«0 simultaneously sat. with both salts dissolve:
0.132 gm. CtHi(NOi)iOTl + 0.36 gm. CtHi(NOi)tOK at o*.
0.352 + 0.44 15 .
0.38 " " +0.23 " " "20*. (Sja)e,i9ot.)
Solubility of Thallium Picsatb in Methyl Alcohol.
(Rabe, z9oz.)
Gms. Gma.
f T10QH,(N(W, Solid Phase. ^ TIOC,H,(N(X). SoKdPluuK.
' per 100 Gms. ' per too Gms. "^^ ^^
CT^H. CH^H.
O 0.39 Red Foim (monoclinic) 45 I -195 Yellow Fonn (tridinic)
18 0.59 « 48 1.265 «
25 0.70 " 50 1.325
30 0.79s " 53 1. 41
35 0.90 « 57 1.54
40 1.02 " 60 1.65
45 1. 17 " 65 1.84
47 I • 265
THALLIUM SELINATE Tl,SeO«.
Solubility in Water.
M
V.
Gms. TliSea
per 100 Gms. nfi.
Authority.
9.3
2.13
Crnttoo, 1907.)
12
2.4
it
20
2.8
(Glauser, tgio.)
80
8.S
M
100
10.86
(Tottoii, 1907.)
THALLIUM SULTATE T1,S0«.
Solubility in Water.
(Berkeley, 1904; see also Crookes; Lan^.)
V,
Solution.
Water.
f.
Solution.
Water.'
0
2.63
2.70
60
9.89
10.92
10
3.57
3- 70
70
II. 31
12.74
20
4.64
4.87
80
12.77
14.61
30
5.80
6.16
90
14.19
16.53
50
8.44
9.21
99.7
IS-S7
18.45
100 nns. H«0 dissolve 3.36 gms. TlsSOi at 6.5^ 4.3 gms. at 12^ and 19.14 gms.
at 100 . (TuttoD» 1907 •)
One liter sat. solution in water contains 48.50 gms. TlsSOi at 20* (Noyes and
Farrel, 191 1) and 54.59 gms. at 25^ (Noyes and Stewart, 191 1).
100 gms. HtO simultaneously sat. with both salts dissolve:
4.74 gms. TljSOi + 10.3 gms. KsSOi at 15^'.
11.5 " " +16.4 " " 62*.
18.52 " " +26.2 " " I00^ (Rabe,i9o>.)
THALLIUM SULFATE 720
Solubility of Thallium Sulfate in Aqueous SoLxmoNS at 25^
(N<vct and Stewart, 19x1.)
Solvent. Satunted Solution,
f ■ ' ' ^ ^^ / ' ■ '^ >
Formula Wts. Formula Wta. Formula Wts. j # Cms. Gms.
Salt Present. Salt Salt Tl^« c^SoL ^^ ""c^*
perUter. per Liter. per Liter. a«- «>»• per Liter, per Liter.
TlNQi o.o99± 0.0996 0.08365 ... 26.51 42.17
NatSOi 0.04995 0.0497 0.1080 1. 0531 7.062 54.44
" 0.20 0.1988 0.1173 1.0754 28.25 59.13
NaHS04 0.1015 o.ioio 0.1161 1.0596 12.12 58.53
H1SO4 0.04967 0.0494 0.1172 1.0540 4.878 59.09
0.09933 0.0987 0.1249 1.0604 9.747 62.95
(t
Solubility of Thallium Sulfate in Aqueous Solutions of Sulfuric
Acid at 25®.
(D'Aos and Fritsche, 1909.)
H,SO..
T1,S04.
Solid Phase.
H,S04.
T1,S04.
Solid Phase
0
0.103
T1,S0«
4.89
0.59
TIHSO.
2.99
0.46
" +Tl,H(S04)t
4.92
0.66
n
4.2s
0.61
T1,H(S04)s+T1HS04
4.78
0.7s
M
4SS
0.56
TIHSO*
4.26
1. 01
M
4-79
0.5s
<i
403
1.08
M
Salt per 100 a
:.Hi0.
Gms. Anhydrous.
8.1
4.61
8.6
Gms. Mob'.
0.0122
0.007
0.0129
THALLIUM DOUBLE SULFATES
Solubility in Water at 25®.
(Locke, 1901.)
Double Sulfate. Formula.
Tl Copper Sulfate TliCu(S04)s.6H20
Tl Nickel Sulfate Tl,Ni(S04)2.6H,0
Tl Zinc Sulfate Tl,Zn(S04)j.6HjO
THALLIUM SULFIDE T1,S.
One liter of sat. aqueous solution contains 0.215 S™* l^i^ ^t 20^. (Bflttger, 1903.)
A diagram and discussion of the fusion points of TltS + S, TltS + Se and
TlfS + Te are given by Pelabon, 1907.
THALLIUM SULFITE TltSOt.
100 gms. H|0 dissolve 3.34 gms. TlsSOt at 15.5^ (Seubeit and Elten, 1892.)
THALLIUM TmOCTANATE TISCN.
Solubility in Water and in Aqueous Salt Solutions.
(Bdttger, Z903; Nqyes, 1890; Noyes and Abbott, 1895.)
One liter sat. aq. solution contains 3.154 gms. TISCN at 20^ 3.905 gms. at 25*,
and 7.269 gms. at 39.75*.
. „ ,^ e , ^. .. Gms. Mob. per Liter. Gms. per liter.
Aq. Salt Solution. t*. *— ttt * ^.o^^r * ' o . * >^o^xt >
Salt. TISCN. Salt. TISCN.
ThamumBramateTlBiOkCeiceu) 39.75 0.01496 0.0221 4.966 5.793(N.ftA.)
ThaDium Nitnte TlNOk 25 O.0227 0.00852 6.04 2.233(N.)
" 25 0.0822 0.00406 21.88 1.064
Potaiifaim Thiocyanate, KSCN 25 0.0227 0.0083 2.208 2.I76(N0
721
THALLIUM VANADATES
THALLIUM VANADATES.
Solubility in Water. (Cameily, 2873; Liebig, z86o.)
V*«^d*te. F«rm«U. Gtns. Vanadate ger loo Cms. HA
At IS'.
Tl. meta vanadate TlVOj
" ortho vanadate TUVQs
" pyro vanadate TUVA
vanadate TluVtOis
it
0.087 (ii"*)
I
o. 20 (14**)
o.toy
At xoo*.
0.21
1.74
0.26
0.29
Gms. Thebaine per
zoo Gms. Solvent.
THEBAINE (Para Morphine) CitHuNOi.
Solubility in Several Solvents.
Solvent. t\
92 Wt. % Alcohol 25
Ether 10
Aniline 20
Pyridine 20
Piperidine 20
Diethylamine
20
0.1
0.71
30
9
2
0.7
Authcvi^.
(Scholtz, 19x3.)
u
THEOBROMINE (Dimethyl Xanthine) C»Ht(CH.)tN40ft.
Solubility in Several Solvents.
Gms. C»Hf (CH^r
N4Q1 per 100 Gms.
Solvent.
Water
tl
«i
it
tt
tt
Aq. 0.25 n HQ
I »HC1
0.1 nNaOH
0.25 n "
1 5.6 per cent Nai(P04)2.Sol.
92.3 Wt. % Alcohol
90 Wt. % Alcohol
DichloreUiylene
Trichlorethylene
Carbon Tetradiloride
Ether
f.
18 .
15-20
18
18
18
18
IS
21
15-20
15
15
b. pt.
b. pt.
0.0305
0.059
0.047
0.083
1.78
4.56
369
0.045
0.02
0.005
0.008
0.021;
0.032
Aathority.
(Paul, 1901.)
(Squire & Caines, X905.)
(Paul, 1901.)
i<
(f
i(
(Briflsemoret, 1898.)
(Squired C^nes, 1905.)
It
(Wester & Bruins, 19x4')
i«
((Sackel. Z897)
TmOPHENE MonoCABBONIC ACIDS a, » and a C«H|SCOOH.
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 fi acid at i8^ 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 0 acid are also given.
THEOPHYLLINE (Theocin) C»Hs(CH,),N40s.H,0.
100 gms. HtO dissolve 0.^2 gm. theophylline at l^-^o^. (Squire & C^aines, 1905.)
100 cc. 90 vol. % alcohol dissolve i .25 gms. theophylline at 1 5-20®. ** "
THOBIUM EMANATIONS.
Data for the solubility of thorium emanations are given by Klaus (1905).
THOBIUM ChloroACETATES.
Solubility in Water at 25^ (Karl. 19x0.)
NaaeofSah. Formula. x^GiS^^igo.
Basic Thoriiun Monochloroacetate (ClCH2COO)iTh(OH)2.HjO o . 0663
Basic Thorium Dichloroacetate (Cl2CHCOO)2Th(OH)2 o . 0887
Basic Thorium Trichloroacetate (CUC.COO)2Th(OH)2 o. 0091
THORIUM BORATE
723
THORIUM BORATE.
The precipitate which results when thorium nitrate b added to a solution of
borax is not a stable compound. ^ Solubility determinations made by four suc-
cessive extractions of it at i8*^ with water, gave the following gms. of material
per lOO gms. HiO; 0.5366, 0.12^0, 0.061 1 and 0.0560. After the fourth ex-
traction, the residue then contamed 10.14% BsOi and after boiling 10 gms.
with 100 cc. of H/) for 6 hrs. and repeating this four times, it contamed 9.63-
9.81 % BsOi. (KaH. 19x0.)
THORIUM mPPURATE Th(C«H».C0.CHs.NH.C00)4.
100 gms. HsO dissolve 0.0318 gm. of the salt at 25^.
(Kaii 19x0.)
THORIUM OXALATE Th(Cf04)t.6H|0.
Solubility in Aqueous Solutions of Ammonium Oxalate at 25*.
(Hauaer and Wirth, 1909a, 191^.)
Gm. Mob. per xooo Gms.
Sat. Sol.
(NHJ,C|0«.
0.00033
0.00072
0.00120
0.00153
0.601 '
I.181"
1.420
i.48ot
ThCQOJ,.
0.00005
0.00012
0.000208
0.00026
0.19s
0.427
0.540
0.563
Solid Phase.
Th(Q0Js.6B^
M
M
mi(Cy)«l,(NH.),.3H^
«
((
l«
Nomiality ^"^^
(^^^ 'IS. sSl'
Solid
Th(Q0«)t.6H«0
o.oi 0.040
o.io 2.203
0.5* 7 . 660 rrh,(C|0«)J(NH4>,.7Hi0
0.5* 10.63
0.5* 15.90
0.5* 17.60
o-S* 17-75
u
«(
u
M
* In these cases the greater part of the ammonium salt entered the solid phase oomfdex 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(Cs04.NH4)4.4H/) is
described by Brauner (1898). It is partially hydrolytically decomposed in
aqueous solution and a solubility determination made by analyzing the solution
ifrom which the nearly pure salt began to crystallize, showed that 100 gms. HtO
contain 90.3 gms. Th(Cj04.NH4)4.4HsO and 9.3 gms. of (NH4)iCj04 (« an addi-
tional i mol. wt.)
Solubility of Thorium Oxalate in Aqueous Solutions of
Hydrochloric Acid.
Results at 17**.
Results at 25^
Results
at 50*.
(Colani, 19x3.)
(Hauser and Wirth, 19x3.)
(Colani. X913.)
Gms. per 100 Gms.
Cone, of Gm. ThOi per
Gms. per
xooGms.
iat. bol.
Aq. HO in xooo Gms. Solid Phase.
Per cent. Sat. SoL
Sol.
ttCL
ThCQOJ,.
' HCl.
ThCCOJ,:
0
0.0017
24 . 8 0 . 100 3Th(QPdtThOi'2Bfi
0
0.0017
1.2
0.0035
37 3.450
41
O.OIO
3.6
0.0061
37.6 3.492
8.4
0.028
4.6
0.0094
12.4
0.057
8.4
0.017
16. 1
0.103
131
0.028
18
0.134
16.2
0.038
19.9
0.169
19.8
0.064
21.6
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(Cs04)iThCl4.2HsO, in Aqueous
Hydrochloric Acid.
(Colani, Z9I3-}
^ Cms. per loo Cms. Sat. Sol. ^ Cms. per xoo Cms. Sat. SoL
w^.
HQ.
Th,(CiOjcu:
12
23
0.12
15
26.3
0.17
12
29.9
0.27
15
32.5
0.48
12
33.1
O.S3
IS
35
1.03
» .
HCl.
Th4(C^J,Cl4.
50
21.2
0.29
50
23
0.34
50
26.8
0.46
50
29.8
0.7s
SO
32.3
I. SI
SO
34.6
2.59
Results are also given showing the effect of oxalic acid upon the solubility of
the above salt in aqueous hydrochloric add.
Solubility of Thorium Oxalate in Aqueous Oxalic Acid Solutions.
Results at 25^
(Hauaer and Wirth, 1919.)
Results at 50^
(Colani, 19x3.)
Gms. per loo Gma. Sat. Sol.
^Cs0«. Th! '
1.7 0.0002
9.3 O.OOI
•3 0.003
Solubility of Thorium Oxalate in Aqueous Solutions of Sulfuric
Acid at 25**.
(Hauser and Wirth, x909a. 19x2; Wirth, 19x3.)
Normality of
Aq. H«Q0«.
I
Sat. Solution
Gm.T1i0^per
zooo Gms. Sat. Sol.
0.0015
0.0030
Solid Phase.
Th(C,04)f6B^
" +H,Cj04.aH^
Normality of
Aq. HaS04.
0.25
0.5
I
2.1
3.2
Gms. ThOi
per xooo Gms.
Sat. SoL
0.07
0.14
0.26
0.418
0.71
Solid Phase.
Th(Q04)9-6H^
((
i<
i<
(I
N/»°g?fe°^ pcr^Gma. Solid Phase.
Aq. HaMJ*. gat. Sol.
4.32
4.9
6.17s
6.885
8.4s
1. 10
1.32
I.S13
1.794
2.473
Th(C,04)a.6Hd0
(I
i<
(I
«<
(Kari, X9XO.)
THORIUM PICRATE Th(CsHiNs07)4.ioH|0.
100 gms. H2O dissolve 0.3052 gm. of the salt at 25^
THORIUM 8BLENATE ThCSeOOi.QHsO.
100 gms. H«0 dissolve 0.498 gm. ThCSeOJi at o* and 1.972 gms. at lOO*.
(Qeve, X885.)
THORIUM SULFATE ThCSOOs.
Solubility in Water.
CRooBeboom, 1890; Demarcay, xSflls.)
Solid
Phase.
M
M
Gms. Th(S04)« per
100 Gms. HaO>
O 0.74 (R) 0.88(D) Th(S04)s4>H20
10 0.98 1.02
20 1.38 1.25
30 1.99s i-^S
40 2.998 2.83
SO S -22(50 4-86
55 6.76 6.5±
o i*o
IS I 38
25 1.85
44 371
Th(SO«)s.8Ha
A o Gms. Th(S04)| per
* * xooGms. HsO.
o i.So(R)
15 1.63
30 2.4s
4S 3'^S
60 6.64
17 941 (I>)
40 404(R)4.S(3S^I>)
50 2.54 I -94 (SS"")
60 1.63
70 1.09 1.32 (7S*')
95 ... 0.71
SoUd
Phase.
Th(SO«)s^HaO
Th(SQi)s.4H^
Additional results for the .8H/) and the .9H/) salt, in fair agreement with the
above, are given by Wyrouboff (1901).
THORIUM SULFATE
724
SCM-UBILITY OF ThORIUM SuLFATB IN AqUBOUS SOLUTIONS OF:
Ammonium Sulfate at i6^
(Barre, 191 z.)
Gms. per igo Gms. H^.
(NHi)tS04. * ThCSOJ,:
2.13 3.361
4.80 5269
10.02 ^.947
16.56 13 330
28 10.359
35.20 9.821
45.14 6.592
4905 S-750
52.88 4.583
69.74 1.653
Solid Phue.
Th(S0«)t.9H/>
Lithium Sulfate at 25^
(Ban«» X913.)
Gms. per 100 Gms. ^0.
tt
tt
" +X.1.4
Z.Zwl
(I
+x*i*i
Z.2.»
x-3-3
M
LiiS04.
O
2.57
4-93
6.98
923
II. 13
13 18
16.12
20.49
25.18
ThCSOJ^
1.722
4.13
6.20
7. 95
9.68
11.05
12.54
14 52
16.02
18.87
1.1.4 - Th(S04)f.(NH4)jSO«.4H«0; 1.2.2 - Th(S04)i.2(NH4)iS04.2H:K); 1.3.3
Th(S04),.3(NH4)tS04.3H/).
Solubility of THORiuif
Results at 16*".
Gms. per 100 Gms. HtO.
K,S04.
O
0.424
1.004
1. 152
1.224
1.283
I 348
I 378
1.487
1.844
3.092
4 050
4.825
Th(S04)t.
1-39
1.667
2.193
3 191
2.514
2.222
1.706
1.637
0.870
0.370
0.070
0.027
0.003
Sulfate in Aqueous
Sulfate.
(Barre, 1911.)
SdidPhue.
Th(S04)9.9H^
Th(S0«)t.K|S04.4B^
Solutions of Potassium
Results at 75".
Gms. per 100 Gms. HtO.
II
II
II
II
Th(S04),.aK«SO«.3H^
II
II
II
Th(S04),.3iKtSO«
II
K«SO«.
O
0.865
1. 167
1. 172
1.270
1.296
1.852
3-"7
4.659
5 348
5.932
7-177
9.706
Th(S04)«.
0.9248
I 137
I 173
1. 121
0.907
0.495
0.297
0.201
0.256
0.170
0.123
0.031
0.022
Solubility of Thorium Sulfate in Aqueous Solutions of Hydrochloric
Acid and of Nitric Acid at 30®.
(Koppel and Holtkamp, 19x0.)
In Aq. Hydrochloric Acid.
In Aq. Nitric Acid.
wt. % na
in Solvent.
Gms. ThCSOJs
per 100 Gms.
Sat. Sol.
Solid Phase.
Wt. % HNO
in Solvent.
Gms. Th(SO«)«
' per xoo Gms.
Sat. Sol.
Solid Phase.
0
2.15
ThCSOdt'SBfi
0
2.15
Th(S04}s.8H/)
4. 55
3.541
tt
517
3.68
II
6.95
3.431
II
10.04
4.20
II
12.14
2. 811
II
16.68
4.84
II
15-71
2.360
II
21.99
4.47
II
18.33
2.199
II
28.33
3.96
M
20
2.IIO
Th(S04)s.4H^
28.51
3.88
II
20
2. 141
II
33 17
3-34
Th(S04)s.4H«0
23-9
1.277
M
38.82
2.51
II
725
THORIUM SULFATE
Solubility op Thorium Sulfate in Aqueous Solutions of:
Sodium Sulfate at i6**.
(Barre» 19x0, 191 z.)
Gms. per 100 Cms. H^O.
Na,S04.
1.094
1.960
2.98
4. II
579
935
12.24
15.36
Th(S0J,.
1.743
2.387
3 962
3. 375
2.136
1.379
1. 169
1.048
SoUd Phase.
Th(S04)t.Na«S04.6Hd0
Sulfuric Acid at 25^.
(Bane, 191 2.)
Gms. per 100 Gms. H^O.
it
(f
u
If
tt
tt
fi
BtSO*.
o
1.072
1. 941
2.821
3.843
5.212
8.0S5
10.105
Th(SO«),.
1.722
1. 919
2.017
2.060
2.061
2.035
1.863
1.702
Sc».ubility of Thorium Sulfate in Aqueous Solutions of Sulfuric Acid
Results at 25^
(Wirth, 19x2.)
Normality Gms. Th(S04)s
Results at 20^ and at the b.-pt.
(Koppd and Holtkamp x9xo.)
of
Aq. H^04.
O
1. 1
2.16
4.32
6.68
9.68
X0.89
15.15
per xoo Gms.
Sat. Sol.
1.593
1. 831
1.488
0.8751
0.4312
O. I04S
0.0636
0.0308
SoUd Phase.
Th(S04)|.9H^
<i
K
(I
H
Th(SO«),.8H^
II
ThCSOOi^HfO
f.
Wt. % Gms. ThgOO,
HtS04 m per xoo Gms.
20
20
20
20
b. pt.
((
((
Solvent.
5
15
25
40
5
10
15
Sat. Sol.
1.722
0.9752
0.3838
0.0103
0.7407
0.4808
0.3882
SoUd Phase.
Th(S04)s.8Hd0
II
II
Th(SO^tJ8B/}
tt
u
wt. %H,S04 Gms.Th(S04)t
in Solvent. xoo Gms. Sat. Sol.
Results at 30^. (Koppeland Holtkamp, 19x0.)
s<*dpi»«- ^SiEi^* ?^S.^i2?sS' Solid Ph«.
o
0.466
0.72
1.468
2.983
4.38
4.97
9.95
2.152
2.055
2.085
2.267
2. 311
2.367
2.323
1. 961
Th(S04)i.8H^
i<
(I
II
If
<f
If
•I
15-03
23.64
32.68
37.80
43.28
45.69
74
80.5
1.484
0.7196
0.3364
0.077
0.0213
0.0047
0.1208
o
Th(S0«),.8Hd0
II
<i
Th(S04)i4H^
tt
It
M
II
THORIUM m Nitrobenzene SULFONATE Th(CeH4.NOt.SO«)4.7HiO.
100 gms. H2O dissolve 61 gms. of the anhydrous salt at 15^. (Hoknberg, X907O
THULIUM OXALATE Tmt(Ct04),.9HsO(?.ioHsO).
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.
100 cc aq. 20% triethylamine oxalate dissolve approx. i .340 gms. thulium oxalate.
(Grant and James, X9X7.)
at
Bromonitrobenzene SULFONATE TmCCsHjBr.NOi.SOi, 14.2)1.-
12H1O.
100 gms. sat. solution in water contain 6.379 gms. of the anhydrous salt at 25^.
(Kata and James, 19x3.)
TH7M0L (3 Methyl 6 Isopropyl Phenol) CaHj.CeHi.OH.CHi.
Solubility in Water. (Seidell, 191 2.)
Ao Gms. Thymol per *«
* • xoo Gms. Sat. Sol. *
25 0.0995 37
30 O.II2 40
35
r.
10
15
20
Gms. Thymol
xoo Gms. Sat.
0.067
0.077
0.088
1.
O.II2
0.126
Gms. Thsrmol
zoo Gms. Sat.
1.
0.132 (i|i-i)
O.141
THYMOL 736
Solubility of Thymol in Aqubous Hydrochloric Acid. (Seidell, i9u^
Nonnality ol ^^^"^ Tbymol per xoo cc Sat. SoL at:
o 0'099S 0.132
O.I 0.0968 (dn^iMM) 0.129
0.5 0.0884 (4i-x*oo9) O.I2I
I 0.0802 (d«-x^x8) O.II2
2.5 0.0612 (<i»-xxM3) 0.093s
5 0.0445 0.0772 U.-xa>8i)
100 cc 90 vol. per cent alcohol dissolve about 300 gms. of thymol at 15^-20^
(Squize and Gaines, z9os*)
Solubility of Thyiicx. in Several Oils. (Sdden, x9zs.)
Gm. Tbymol per xoo Gms. of:
r.
OGve Peanut Cod Liver Liquid CastOT Cottonseed Linwerd
Oil. Oil. OiL Petrolatum. OO. OiL OiL
10 46.2 73 SO 31 81.2 s6.2 62.3
IS SO. I 73-8 S2 3-9S 902 64 63.1
20 s6.2 74.6 ss^S S-6 loi.s 74.2 65.1
2S 66.9 76.4 63.1 9.78 116. 5 89.4 69
30 84. S 832 77 16.3 137 113. 7 78.3
3S m 106.7 102 25.5 165 146.5 100
37 124.3 130.5 116.5 29.9 180 166.5 116.5
40 151. 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 thjrmol in the several oils are also given.
Distribution of Thymol between Water and Oils at 25^ and at 37^
(Seidell, X9Z2.)
Water + Olive Oil
•
Water + Cod Liver Oil.
Water + Peanut Oil.
Gms. Thymol per xoo cc.
OU H^
fL.
Gms. Thymol per loo cc
^ ft.
Gms. Thjrmol per 100 cc
oa HjO
^^
r.
oa H,0
Layer (4)- Layer (c^).
<w
Layer (4) Layer (O*
««f
Layer (4). 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 46.3s
427
0.1099 43 -81
399
37
0.0807 33.48
41S
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 thjrmol and sulfuric acid are given by
Kendall and Carpenter (19 14).
Results for thymol + bromotoluene are given by Patemo and Ampola (1897).
TIN Sn.
«
Distribution of Tin between Aqueous Hydrochloric Acid and Ether at
Room Temperature. (Mylius, x9xx.)
When I gm. of tin as the chloride, SnCli, 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% HCl, 17 per cent; with 15% HCl,
28 per cent; with 10% HCl, 23 per cent; with 5% HCl, 10 per cent and with
1% HCl, 0.8 per cent of the tin.
727 TIK CHLOBIDS
TIN CHLOBIDS (Stannous) SnCls.
100 gms. HsO dissolve 83.9 gms. SnClt at o^ and 269.8 gms. at 15^ Sp. Gr.
of Solutions 1.532 and 1.827 respectively. (Engd, 1889; Michel and Krafft, 1851.)
Solubility of Stannous Chloride in Aqueous Solutions of
Hydrochloride Acid at o^.
(Eogel.)
liniicram Mols.
Solution
per 10 cc.
Sp. Gr.
of
0 • -j^
Grams per xoo cc.
Solution.
HQ.
iSnOt.^
Scluticn.
HQ.
SaQa.
0
74.0
• I 532
0.0
70.26
6.6
66.7
1.489
2.405
63-33
13 54
63 -75
1.472
4.93s
60.52
24.8
68.4
I 524
9.04
64.9s
34-9
81.2
1.625
12.72
77.11
40.0
94.2
1.724
14.58
89.45
440
117. 6
1.883
16.04
III. 7
49.4
147.6
2. 114
18.01
138.6
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. SnClt at 18^. (di^ » 1.6.) (Naumann, 1904.)
100 gms. ether dissolve 11.4 gms. SnClj.2HiO at o*-3^.5*.
100 gms. ethyl acetate dissolve 31.2 gms. SnClt.2HiO at — 2^ 35.53 gms. at
+22^ and 73.44 gms. at 82^ (von Laazynski, 1894.)
100 gms. ethyl acetate dissolve 4.46 gms. SnClt at 18^. d]^ of the sat. solution
» 0.9215. (Naumann, 1910.)
100 gms. 95 per cent formic acid dissolve 4.1 gms. SnCU at I9^ (Aachan, 1913.)
Freezing-point data for mixtures of SnClt + ZnCls are given by Herrmann
(1911).
TIN CHLORIDE (Stannic) SnCU.
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 SnCU, in terms of CI, which
entered the xylene layer was determined. The amount of Sn and CI in the
xylene was found to correspond to SnCU.
Results for Xylene + SnCl4.5HtO. Results for Xylene + SnCl44HtO.
Gms. Q per 100 Gms. Gms. CI per xoo Crms.
Xylene
Layer, e',
0.08
0.18
0.33
0.68
Per cent CI in SnCl4.5HiO - 40.38. Per cent CI in SnCl4.4HiO » 42.37.
Results for Xylene + SnCl4.3HiO.
Gms. Q per xoo Gms.
Xylene p*
Layer, c'.
9-93 4.4
9.32 4.6
10.56 4.1
10.03 4.2
Per cent CI in SnCl4.3HiO » 45.12.
r.
Aq.
Layer, c.
66
40.3s
80
39. 95
97. S
40.24
III
40.27
c
f.
Aq.
Layer, c.
Xylene
Layer, c\
c
c''
504. 4
66
41.9
0.92
45. 3
228.5
80
41.91
1.56
27
122. 1
100
41.85
2.52
16.7
59.3
III
41.68
3.23
12.9
80
Aq.
Layer, c.
43-2
94
42.54
100
42.64
III
42.31
TIN HYDBOZIDS 728
TIN HTDBOZIDE (Stannous) Sn(OH)s.
One liter of the saturated solution in water contains 0.0000135 gm. mob.
Sn(OH)t at 25^ (GoldBchmidt and EckhanU. 1906.)
Solubility of Stannous Hydroxidb in Aqueous Sodium Hydroxidb
Solutions at 25®.
(Goldschmidt and Eckhardt, 1906.)
The authors desired to ascertain whether the mono, NaHSnOt, or the disodium
salt, NatSnOt, predominates in alkaline tin hydroxide solutions. Given amounts
of carefully prepared tin chloride, made from tin and HCl, 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)t, analyzed.
Gm. Mols. per liter.
»
Gm. Mob. per liter.
Total Na. NaHSnCV
NaOH.
Total Na.
NaHSnOi.
NaOH.
0.00451 0.0009845
0.003525
0.02250
0.00838
O.OI412
0.00680 0.00218
0.00462
0.02788
0.01038
0.0175s
O.OII49 0.003495
0.007995
0.02940
0.00874
0.02066
0.02143 0.006935
0.01449s
0.03012
0.00865
0.02147
0.02143 0.00660
0.01483
0.03036
0.01082
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.
CRubc&baoer, 1902.)
Cms. per 90 cc.
SolutioQ.
Md.
Dilution of the
NaOH.
Gms. per so cc. "^^
Solution. Dilntioii «W the
* Na. Sn.
' Na.
Sn.
NaOH.
0 . 2480 0 . 1904
1.86
0.8326
0.5560
0-S5
0.3680 0.2614
■ I -^5
0.9661
0.7849
•0.48
0.6394 0.4304
0.72
2.1234
1.8934
0.23
TIN IODIDE (Stannous) Snis.
Solubility in Water and in Aqueous Hydriodic Acid.
(Young, 1897.)
t*. Gms. Snia per xoo Gms. Aqueous HI Solutions of:
o%-HjO.
5^3%.
9A>%.
iS.a%.
20-44%.
^a£>%-
304%.
36.83%.
20
0.98
0.20
0.23
0.60
1. 81
4.20
10.86
2S-3I
30
1. 16
0.23
0.23
0.64
1. 81
4.06
10.28
23.46
40
1.40
0.33
0.28
0.71
1.90
4.12
10.06
23 15
so
1.69-
0.46
0.38
0.82
2.12
4-34
10.3s
23.76
60
2.07
0.66
o-SS
I .11
2SI
4.78
11.03
24.64
70
2.48
0.91
0.80
1-37
2.92
S-43
11.97
25.7a
80
2.9s
1.23
I 13
1.83
3 70
6.38
13-30
27.23
90
3-46
1.65
I 52
2.40
4.S8
7.8a
ns^
29.84
100
4-03
2.23
2.04
3-^3
S-82
9.60
• • •
34.0s
Tm, IODIDE (Stannic) Snl4.
Solubility in Organic Solvents.
(McDermott, 19x1.)
Solvent.
Carbon Tetrachloride
22.4
Sp. Gr.
Sat. Sol.
I.S9
Chloroform
Benzene
SO
28
20.2
1.63
I. SO
0.95
Gms. Snl« per
xoo Gms. Sat. SoL
12.50
8.21
12.65
729 TIN lODZDS
SOLUBIUTY OF STANNIC lODIDB IN CaRBON DISULFIDE.
(Sneider, z866; Arctowaki, x895-'96.)
-ii4*.S. —94*. -89*. -84*. —58*. Ord. temp.
Gms. Snl4 per 100 (ims.
Solution 9.41 10.65 9-68 10.22 16.27 59.2(8)
100 gms. methylene iodide, CHsIt, dissolve 22.9 gms. Snl4 at 10^. Sp. Gr. of
solution » 3.481. (Retgers, 1893.)
TIN OXALATE (Stannous) Sn(COO)t.
100 gms. 95 per cent formic acid dissolve o. 16 gm. Sn(COO)t at 19". (Aschan, 19x3.)
TIN TetraPHENYL (Stannic) Sn(C6H«)4.
Freezing-point data for Sn(C«H«)4 + Si(CeH»)4 are given by Pascal (1912).
TIN SULFATE (Stannous) SnSOi.
100 gms. H^ dissolve 18.8 gms. SnS04 at 19" and 18.1 gms. at loo^ (Marignac.)
TOLUENE CiHtCH,.
Solubility in Sulfur.
• Figures read from curve, synthetic method used, see Note, page 16. (Akzejew, z886.)
Gms. C»HaCH| per 100 Gms. ^ Gms. CeHtCHt per 100 Gma
f.
' s
Toluene
Lafer.
Layer.
100
3
73
no
4
7»
120
5
68
130
7
66
140
95
63
* • ' s
Layer.
Toluene
Layer.
150 12.5
160 16
59
53
170 22
47
175 25
178 crit. temp.
34
43
NitroTOLUENE 0 CeH4.CHt.NO1.
Reciprocal Solubility of 0 NrrRoroLUENS and Water.
(Campetti and Delgrosso, 19x3.)
The original results were plotted and the following figures read from the
curve.
Gms. 0 Nitrotoluene per xco Gms.
f.
245
250
25s
360
263 -5
Gms. 0 Nitrotoluene per xoo Gmi
f.
150
175
200
225
240
^Ridi
Layer.
I
1-5
3
6.5
10.5
Nitrotoluene
Rich Layer.
98
96
93
89
84
H^ Rich Nitrotoluene '
Layer. Rich Layer.
13 81
16 78
20 72
29 63
crit. t. 43
100 gms. 95 per cent formic acid dissolve 13.25 gms. p C«H4.CHt.NOs at 20.8^
(Aschan, X9Z3.)
TrinitroTOLUENE 2,4,6 C6Hs.CHt(N0t)t.
100 gms. HsO dissolve 0.021 gm. C6Hs.CHt(NOt)t at 15^ and 0.164 gm. at I00^
100 gms. alcohol dissolve 1.6 gms. C6HsCHt(N0i)t at 22^ and 10 gms. at 58^.
(Capisarow, X9X5.)
TOLUENE SULFONAMINE8 0, m and p.
Solubility of Each in Water at 25®. (Holleman and Caland (x9xx.)
Compound. ^"^ ^^^sT ^^
Amine of (7 Toluene Sulfonic Acid 1.624
" " m " " " 7.812
TOLUIMI 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 Lma, 1907.)
Bromotoluene + P Xylene (Pateno and Ampda, 1897.)
" +Veratrol
" + Tribenzylamine
p Nitrotoluene + <x Ortho Nitrotoluene (HoOeman, x9X4-)
M -La" *• "
" + 3, 4 Dinitrotoluene (Giua. 29x4. 1915.)
+ 2,6 " (Giua. 2915.)
+ 2,4.6 "
" + m Nitrotoluene (Holkman and van den Arend. 1909.)
" + Urethan (MaacareUi. 2908, 2909.)
2, 4 Dinitrotoluene + 2, 6 Dinitrotoluene (Giua, 29x4, 29x5.)
" 4- 2, 4, 6 Trinitrotoluene ((3iua. 29x5.)
2.6 " + '* " (Giua. X9X4. 29x5.)
a Trinitrotoluene + p Amino Acetophenone (Giua. x9x6.)
" 4- 7 Trinitrotoluene ^ (Giua. X91S.)
o Toluene Sulfochloride + p Toluene Sulfochloride (HoUeman and Caland, xgxi.)
Binary Mixtures of Isomeric Tribromotoluenes (Jaeger. 2904.)
" " Chloronitrotoluene8^**"'»'»'^\^**'»»""^~*"
Axend, X909.)
TOLUIC ACIDS (Monomethyl Benzoic Acids) CHt.CeH4C00H.
Solubility in Water at 25*.
(Paul, 1894.)
... CH«.C«E[4.(XX)H per Liter Solution.
Grams. Millimols.
Meta Toluic Acid 0.9801 7.207
Ortho Toluic Add 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 S™* P toluic acid at 25^
(Sidgwic^, X9X0O
Solubility of Toluic Acids (Each Separately) in Water at Various
Temperatures.
(Sidgwick, Spurrell and Davies, X925.)
The determinations were made by the synthetic method, see p. 16; melting-
point of 0 toluic add — 102.4®, of m add = iio.s* and of p add = 176.8®. The
triple point (solid phase [jresent) for the 0 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 qi.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 200 Gms. Sat. Sol. Gna. per 200 Gms. Sat. Sol.
r.
• Toluic
M Toluic
^Toluic
r.
0 Toluic
m Toluic
^Toluic
Acid.
Add.
Acid.
Acid.
Acid.
Add.
80
2.03*
1. 16*
« ■ •
140
9.25
5.77
4.30^
99
2.42*
1. 54
• • •
ISO .
13.7
8.40
9.33
100
2.97
1.98
i.i6*
159. 1 cnt t.
• • •
• • •
00
110
3.71
2.52
1.36*
160
30
19.4
120
S-io
3 24
1.75*
161 . 1 crit. t.
00
. . •
130
6.93
430
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 thb Solubilities of Toluic Acids (Separately Determined)
IN Water and in Olive Oil at 25®.
(Boeseken uid Waterman, X9xx, 19x3.)
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.
... „ ,. . Solubility in Olive Ofl
Acid. Ratio of c 1 wi-> » w «. — *
Solubility in Water
0 Toluic Add 40.5
m 21
p " " 29.5
100 gms. 95% formic acid dissolve 2.09 gms. o toluic acid at 20.8^. (Aacfaan. xqxj.)
Freezine-point data for mixtures of 0, 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).
TOLUmiNE CeH4CH,.NHs.
Solubility in Water.
(Vaubel, 1895; Lowenhers, 1898.)
Gms. Gms.
^» C^H^CHtJnia Solid «• CACHiNHa Sdid
per xooo Phase. * per xooo Phase.
Gms. HfO. Gms. HsO.
30 16.26 liquid ortho T. 20.8 7-39 PftraT.
20 0.15 OrthoT. 26.7 9.50 ••
20 6.54 PtoaT. 31.7 11.42 "
One liter sat. solution in water contains i^ gms. 0 toluidine at 25^.
One liter sat. solution in i n aq. 0 toluidine hydrochloride, contains 30 gms.
o toluidine at 25*^. (Sidgwick, 19x0.)
The following results for p toluidine, differing considerably from the above,
are given by milker (1890).
t^ 22** 30** 36.7** 44^ 57-5'' 69^
Gms. p Toluidine per loo Gms.
Sat. Sol. in Water 19.6 26.9 35.4 44.5 51.4 58.9
Solubility of Para Tolutoinb in Ethyl Alcohol.
(InteipoUted from origiiial results of Speyers, Z903O
Wt. Mols. per Gms. per
t". of 1 CC. 100 Mob. 100 Gms.
Solutioo. CsHiOH. CAOH.
20 0.9265 47 -O IIO-O
25 0.9360 56.0 132.0
30 0.9460 66.0 156.0
100 gms. pyridine dissolve 126 gms. p toluidine at 20^-25^. (Dehn, 1917.)
100 gms. aq. 50% pyridine dissolve 96.1 gms. p toluidine at 20^-25^. "
Distribution of Para Toluidine Between Water and Carbon
Tetrachloride.
(Vaubd, 1903.)
Om.ytM6b^ Volume ol Solvit.. Gm,. Ca(CHJNB^ » In:
Uaed. ly) Lsyer. CCI4 Lsyer.
I 200 cc. H2O+ 100 CO. CCI4 o . 1406 o . 8594
I 200 oc. HjO+ 200 CC. CCI4 o . 0666 o . 9334
Wt.
Mols. per
Gms. per
*•.
of ICC.
xoo Mols.
100 Gms.
Solution.
CsHsOH.
CsHiOH.
0
0.8885
20.72
48.1
5
0.8982
26.0
60.0
10
0.9080
32.0
74 0
IS
0.9180
38.6
90. c
TOLUJLDJLNE 732
DisTUBunoN OF Of m and p Toluidinb bbtwbbn Water anb
Bbnzbne at 25^
(Fanner and Wuth, 1904.)
w% TV! r^ _* Conc« 10 CaBm
• Cone in H^'
0Toluidine 13.4
m " 19. I
P " 24.1
Aceto TOLUIDINE p CHtC6H4NH.C>H^.
Solubility in Mixtures op Alcohol and Water at 25^
(Hollmun and Antuach, 1894.)
V/J 9/ Cms. per Sp. Gr. %t* or Cms. per Sp. Gr.
J^^ xooGms. of X^j^ xoogS. of
'^*****- Solvent. Soludona. Alcohol. Solvent. Solutioos.
100 10.18 0.8074 50 1.92 0.9306
95 10.79 0.8276 45 I. 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 5.81 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.
T&iPUBNTLAMINE, T&iFUENYLPHOSFUINE, etc.
F.-pt. data are given by Pascal (1912) for the following mixtures:
Triphenylamine + Triphenylarsine Triphenylarsine + Triphenyl Stibene
Triphenylamine -|- Triphenylphosphine Triphenylarsine 4- Triphenylbismuthine
Triphenylarsine -(- Triphenylphosphine Triphenylphosphine -j- "
a and ^ TJEUTmOACSTALDIHTDE, (CH,CHS),.
aand fi TRITmOBENZALDIHTDE, (CeH»CHS),.
Solubility of each (Determined Separately) in Several Solvents
AT 25'.
(Suyver, 1905.)
Gms. per zoe
» Gms. Solvent
Ether
Ethyl Alcohol
Methyl Alcohol
Acetone
a (CHaCHS),.
IS 58
3.86
4.04
20.96
fi (CHiCHS)..
13 67
3-97
3.89
18.31
« (CACHS)*.
1.09
0.20
0.17
2. 45
fi (CACHS)..
0-37
0.04
0.04
1. 12
Chloroform
Carbon Disulfide
57- 59
25 SO
51-22
20.75
II. II
5.81
0.20
0.22
Benzene
36.40
26.98
6.08
0.014
Ethyl acetate
17. S2
15.48
2.05
0.93
Data for the solidification points of mixtures of a and fi trithioacetaldehyde
are also given. Similar data for mixtures of a and fi trithiobenzaldehyde could
not be determined on account of decomposition with production of resins.
TROPIC ACID (a Phenylhydracrylic Acid) * and /, C«H».CH(CH,OH)COOH.
100
100
gms. sat. solution in HtO contain 1.975 gms. of the i acid at 20^ ) (Schlossbeig.
gms. sat. solution in HtO contain 2408 gms. of the / acid at 20**. ) 1900.)
^ 733 TURPENTINE
TUBPENTINE OIL
Solubility in Ethyl Alcohol.
(Vezes and Mouline, 1904, 1905-06.)
Spirit of turpentine and absolute alcohol are miacible in all proportions and the
mixture may be cooled to a very low temperature without ceasmg 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.
CtHsOH per i gm. aq. alcohoH and spirits of turpentine and for mixtures of 95
vol. % alcohol ( — 0.924 gm. CsHsOH per i gm. aq. alcohol) and spirits of tur-
pentine.
Results for 98 Vol. % Alcohol. Results for 95 Vol. % Alcohol.
40 ^e Gms. 98 VoL x* » Gms. 98 VoL ao ^t Gms. 95 Vol. xe # Cms. 95 VoL
**°°- Mixture. ^°- Mixture. ^^- fixture. ^^- 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
— 20.9 9.5 -30 48.2 S3 7.2 16.3 61.4
— 18,1 13.2 —45-3 S^ 53-1 IO-2 — iSS 7^.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.
URANTL Potassium BUTTRATE UOi(C4H70s)2.KC4H70s.
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
KC4H704 is 2.10 gms. UOi(C4H70i) + 0.38 gm. KC4H7O1 per 100 gms. solution.
The atomic relation being i : 0.64. (Rimbftch, 1904.)
URANTL Ammonium CARBONATE U0iC0t.2(NHi)sC0t.
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.
f.
Gms.
per 100 Gms.
Sat. Sol.
Mol. Ratio.
U.
CQ|.
NH,.
'u"
: CQi :
NH,.
18.6
2.71
1-54
0-79S
I
3 08
4.10
36 s
309
2.29
1. 188
I
4.01
S-3S
48.3
3 03
2.71
I -35
I
4. 95
^'35
62
• • •
3.17
1.62
• • •
• ft •
• ■ «
87 -3
3 -95
3 96
2.027
I
S-42
71s
Theoretical molecular ratio for U0iC0j.2(NH4)iC0i = 1:5:4.
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 U02COs.2(NH4)sCOi are contained in
100 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.).
UBANYL CHLORIDE UOiCls.3HsO.
100 gms. HtO dissolve 320 gms. UOtCls at i8^ (Mylius and Dieu, 1901.)
URANTL CHLOBIDU
734
Solubility op Uranyl Ammonium Chloride, U. Tbtra Mbthtl Ammonium
Chloride, U. Tetra Ethyl Ammonium Chloride, U. Caesium Chloride, U.
Rubidium Chloride, and U. Potassium Chloride in Water.
(Rimbach, 1904.)
(«, Gbm. per 100 Gms. Sat. Sol. Atomic ReUtioa in Sol. Solid Pbaae.
Fonnula of Doubk
Salt.
U0yClf3NH«a.2H^
U0hClt.aN(CHi)«a
U0aCl|.3N(CaHa)«a
uo,ci|.2Csa
U0bCl|.2Rba.jH/>
UO^-aKCLaHdO
ff
«f
l€
U
U
i$
If
IS 4O.67U0i+3.SiNH.+i9.isa lUO*: 1.S9NH4: 3-590 ^^M^NHia
«9.«
80.7
«7.i
80.7
29.75
34.8
80.3
0.8
149
17. 5
35
4Z.5
so
7«.5
78.5
19^5
30.23
I5X>2
15 -za
22.11
37-z8
30.66
38.57
33-71
37.36
3501
35»7
34.18
3419
33-55
35.a6
i<
it
tt
II
«l
«l
u
it
(I
M
II
II
--1044CU -4i-a4*
+ZO.<2Clt —41 .91*
-- 7.8iClt -37.i5t
-- 7.78CI1 -37a3f
+22.5 Cs
- -16.6 Rb
- -x9.zRb +XS.8CIJ1
3.86K
-37I5T
-37a3t
"56.04?.,
+X3.8CII
-f 13.593
--13.51CI
-4-14.500
--15.260
--iS.9aCl
- -16.560
- -i7.asO
--17.44CI
- -18.340
K
S-27K
• • ■ ^^
7.39K
• ■ • ^^
9.28R
9-95K
xUOh: 4.oaO
lUO^: 3-98O
lUQi: 3.97a
lUOi: 3.94a
lUO^: 3.070
zUOh: i.96Rb:
3.900
lUOh: z.98Rb
■iM°
lUOh: 3.69a
lUO^: 3^60
1.06K
lUO^: a.960 :
0.96K
lUO^: 3.33a :
X.33K
lUOi: 3.44O :
X44K
lUOi: 3.71O :
X.71K
lUO^: 3.85O
x.8<K
1.96K
iU0,:3.96O:
lUO^: 3.95a :
1.95K
Dottbknlt
M
II
II
If
H
Tbe double aalt
is decomposed
by water at
temperatures
below 60*.
Double nit
II
uohO«.2N(CHi).o. t u0hai.N(CA)4a. t uO|Ci..2Csa.
I -57.9 8msrUQiai.aRbC^ H -65.8 gms. U0ka|.2RbC^
URANYL Sodium CHBOMATE 2(UOt)Cr04.NasCr04.ioHsO.
100 gms. sat. aqueous solution contain 52*52 gms. 2(UOi)Cr04NasCr04 at 20^
(Rimbach, 1904-)
URANTL lODATE UO,(IO,)t.
Solubility of the Different Crystalline Forms in Water at I8^
(Artmami, 191 2-13.)
Appearance of Ciystala.
UQi(IQs)s.H20 Type I warty, later prismatic needles
** Type n pyramids, sphenoids
UQi(I0,),.2Hrf)
Gms. UQiaCVt
per zoo Gobs, a/),
0.1049
O.I214
0.2044
U&ANYL NITIUTE UO,(NO,)t-6HiO.
SOLUBILFTY IN WaTER.
(Wasilieff. 1910.)
f.
— 1.6
— 2.1
— 2.9
- 6
- 7.9
— II. 2
-18. 1
— 12. 1
Gms.UOh(NO,)t
per zoo Urns.
Sat. Sol.
10.83
12.24
17.19
26.20
32.53
3709
43"
45-53
Solid Phase.
Ice
'< +U0^0^s-6H|0
U0,(N0k)t-6H«0
r.
— 2.2
O
5-5
".3
21. 1
25.6
36.7
45-2
SI. 8
Gm8.U0hgf0k)t
per zoo Cms.
Sat.SoL
43.77 .
49 46
50.5s
52.88
55.98
57.17
61.27
65.12
67.76
Solid Phase.
U0^0^6H«0
M
(deCoiiiiick,i9oa)
M
100 gms. abs. acetone dissolve 1.5 gms. U0i(N0i)i.6Ht0 at 12^.
100 gms. 85% alcohol dissolve 3.3 gms. UOt(NOi)s.6HiO at 12
Data for the densities of uranyl nitrate solutions in water and other solvent!
are given byde Coninck (iQOo),
«
59
l(
80.7
UO,(NOi)j.CsNQi
16
UO,(NQi)i.KNQi
o.S
«
13
<(
25
tt
45
<(
59
«
80,6
UQi.(NQi)f.RbNOi
25
u
80
735 U&ANTL NITRATE
SOLUBSLITY OF UrANYL NiTRATB IN EtHBR.
(Lebeau, 19x1.)
When a large excess of uranyl nitrate is shaken with ether at 7^, two liquid
layers are formed. The ethereal layer contains 59 gms. UC)s(NOi)t 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 UOt(NOs)t.6HsO were mixed
at room temperature, therefore, indicating that solution is accompanied by com-
bination and elimination of the water of the salt.
U&ANTL DOUBLE NITRATES.
Solubility of Uranyl Ammonium Nitrate H- Uranyl Nitratb; U. Caesium
Nitrate + Caesium Nitrate; U. Potassium Nitrate + Potassium Nitrate
AND U. Rubidium Nitrate + Rubidium Nitrate in Water.
(Riznbftch, Z904O
Formula of SiUt. f. ?"^- P«^ '«> 0°^- S>t. SolutJon. AtomAcReUttion
UOi. Total Salt. "> Solution.
UQi(NQi)j.NH4NQi 0.5 29.7i + 2.92NH4= ... lUd: 1.47 NH4: 3.47 NQi
24.9 36.46 + 3.54 " -68.95 " :i.46 " :3.46 "
44.37 + 2.90 " = ... " :o.98 " ;2.98 "
80.7 44.95 + 2.98 " =78.95 " .'I " :3 "
i6 31.39 + 6.59 Cs ="55-4 " :o.44Cs
0.5 31.98 + 1.72K = ... " .-2.37 N(^:o.37K
33.40 + 2.72 " = ... " :2.57 " :o.57"
37.07+4.01 "♦ =64.82 " :i.6o " :o.76"
42.18 + S.16 " «... " 12.84 " :o.84"
41.65+6.03 " = ... "13 " :i "
43.71 + 6.38" -80.1 " 13. 01 " :i.oi"
35.41 +4-65 Rbt =59.60 " :i.4o " :o.45Rb
34.66 + 11. 01" =69.49 " :3 " ii.oi "
• + 23.SNO,. t + 19.74NO,.
URANTL OXALATE UO1.CtO4.3H2O.
100 gms. HsO dissolve 0.7401 gm. UOiCi04.3HtO at 25^ (Dittrich, 1899.)
Equilibrium in the System Uranyl Oxalate, Ammonium Oxalate
and Water.
(Colani, 191 7.)
Results at 15^. Results at 50^
Gms. per xoo Gms. Gms. per 100 Gms.
Sat. Solution. Solid Phase, Sat. Sqlution. Solid Phase.
UOiCiO*. (NH4),C04. tJQiCiO*. (NHO,C,04.
0.47 O VOtCfiisW} I O UOb.CO4.3H1O
7.19 2.14 « +(NH4),(UO0i(C|O4),.3HiO 5 . II 1 . 36 " +(NH4),(UQ0t(CiO4),
8.78 2.99 (NH4),(UOs)(C04),.2H,0+ " 19.89 8.52 (NH4),(UQ0(C,O4),+ "
9.66 6.43 " +(NH4),C04.H,0 23.82 15.90 " +(NH4),Ci04.H|0
O 3.69 (SHdtCfiiMfi O 9.36 (NH4),Cj04.H^
Two determinations at 75" are also given.
Equilibrium in the System Uranyl Oxalate, Potassium Oxalate
AND Water.
(Colani, z9x6a.)
Results at 15"". Results at 50".
Gms. per 100 Gms. Gms. per 100 Gms.
Sat. Sqlution. Solid Phase. Sat. Solution. Solid Phase.
UOiQO*. K,C|04. tJOiPA. KtC,04.
0.47 O U0,Ci04^H*0 I O U0bC,0«.3H*0
1 . 34 0 . 42 " +K,(UQ0i(CfO4)i.4H^ 3-45 I • " " +K,(UO0j(CfO4),.4HiO
3.89 1.83 Kt(UOs)(C04),.3*HjO+ " 9.82 4.83 K5(U0s)(C0A+ "
3 . 76 1.85 " +K«(UOO»(C,04),.ioH,0 9 . 59 5.61 " +K.(U0s),(C04),.ioH|0
O.IO 24.30 K,C,04JV)+ " 1-22 32.65 K,C04.Hj0+
O 24*09 X«C|Q«.H/> O 32.75 X«CAW>
UBANTL OXALATE
736
Gms. UOk.CiO4.3H/>
per xoo cc. Sat.
Solution.
Solubility of Uranyl Oxalate in Aqueous Sodium Oxalate at 25**.
(Dittrich, Z899.)
Gmi. NatC|04
per xoo cc.
Solution.
0.6706 2.0125
0.33S3 0.9867
0.2235 0.6059
URANTL Ammonium PROPIONATE 2UO,(C,HBOt)t.NH4CtH60t.3H^ .
URANYL Potassium PROPIONATE U0t(C.H»0t)i.KCsH»0t.
100 gms. aq. solution contain 16.48 gms. 2UOs(CiH50t)t.NH4CsH60s at 29.8**.
100 gms. aq. solution contain 2.362 gms. U0s(CtH«0s)s + 0.82 gm. KCsHsOs
at 29.4 , atomic relation, i: 1.29. (Rimbach, 1904-)
URANTL SULFATE UOtS04.3HsO.
Solubility in Several Solvents.
(de Coninck, 1901, 1903.)
Gms. UQ1SO4.-
Gms. U0iSO4.-
Solvent
f.
3H1O per zoo
Gms. Solvent.
Solvent.
f.
3H^ per xoo
Gms. Solvent.
Water
13-2
18.9
Cone. HBr (J=i.2i)
12
16.8
Water
^SS
20.5
Cone. HNOs
12
9.1
16.2% Alcohol
10
12.3
Cone. 112804(^=1.138)
13
24- 3
85% Alcohol
16
2.6
I Vol. HCl+i Vol. HNO,
16
18
Cone. HCl
13
30
Sdenic Acid (^=1.4)
15
27
URANTL Potassium SULFATE UOtSO4.KsSO4.2H1O.
100 gms. sat. aq. solution contain 10.41 gms. UO1SO4.KSSO4 at 25^ and 23.13
gms. at 70«5^> (Rimbach, 1904.)
Solubility of UOjSO4.2K1SO4.2H1O + UO1SO4.K1SO.2H1O in Water.
Gms. per 100 Gms. Solution. AtcHnic Relation in Sol. Mol. % in Solid Phase.
i/oT
f.
14
SO
80
UO,.
0.85
6.70
14.29
K.
4.19
8. IS
8.54
SO4.
S.71
12.37
15- S3
K. SO4.
I : 35.75 : 18.88
I : 5.20 : 8.40
I : 4.13 : 3.06
Mono Salt. Di Salt.
29 71
76 24
12 88
SULFATE
18
25.6
37
48.2
62
Gms. U(S04)i
per 100 Gms.
Sat. Sol.
10.17
13.32
19.98
28.72
36.8
(OUS) U(S04)|.
• Solubility in Water.
(Giolitti and Bucd, 1905.)
Gms. UCSOOs
t^. per 100 Gms.
Sat. Sol.
93 63.2
24 9.8
37 8.3
48.2 8.1 (7.8)
. 63 7.3
Solid Pbase.
it
It
It
Solid Pbase.
U(S04),.8HaO
U(S04),.4HiO
K
If
tt
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
Dilute HCl (i : 4)
Dilute HNO, (1:4)
Gms. Gms.
*•• K.-^ solvent- *•• S^"?^'-^
Solvent. Solvent.
II 23.2 Dilute Selenic Acid (i : 4) 11. 4 21.7
9 17.2 Dilute H1SO4 (1:4) 10 15.6
10.5 x8.2 Dilute Alcohol (1:4) 11-3 12.3
737
UBSA
UBSA CO(NHi)s.
Solubility in Water and in Alcohols.
(Campetti, 1903; Speyen, 1902.)
Note. — Speyer's original results are in terms of Mols. CO(NHi)t per 100 mols.
H^ at irregular temperatures.
In Water. In Methyl Alcohol. In Ethyl Alcohol,
Gms.
Gms.
A A
Wt. of X oc.
Gma. CO(NHs)s
per
Wt. of X cc.
COCNH,),
Wt. of X cc.
CO(NHj),
t*.
Solution.
100 Gms. HaO
.
Solution.
per too Gms.
CHsOH.
Solution. ]
per xooGms
'
.QsHsOH.
0
1. 121
5S-9
. ■ ■
0.861
13.8
0.8213
2-5
10
1-134
66.0
85-
o(C)
0.863
16.0
0.814
35
20
1. 146
79.0
108.
,2(C)
0.869
20.0
0.809
S-o
30
I 156
93 0
0.876
24.0
0.806
6.5
40
1. 165
106.0
0.890
30 0
0.804
8-5
SO
I -173
120.0
0.908
37 0
0.803
10.5
60
1. 180
132.0
0.928
47 0
...
13.0
70
1. 187
145 0
1^1 «
• t
• ■ a
A
• t •
...
_^ __ -0
17.5
100 gms. abs. methyl alcohol dissolre 21.8 gms. CO(NHOs at 19.5^.
100 gms. abs. ethyl alcohol dissolve 5.06 gms. C0(NHs)2 at 1 9.5^. (de Brayn, 1905.)
Alcohol.
Methyl Alcohol
u
u
€1
Ethyl Alcohol
u
li
u
u
Propyl Alcohol
€1
€t
U
it
Solubility of Urea in Alcohols.
(Timofeiew, 1894.)
Gms. C0(NHs)t
t*. per xoo Gms.
Solvent.
— 12 II
o 14.2
19 20.9
40 36.4
62 66.6
71 107.4
— 9 2.69
o 3.26
18 5
41 9-45
60 16.3
81 30.8
o 1.65
20 2 . 56
40 5.12
60 7.72
80 12.28
98 18.06
Alcohol.
Isopropyl Alcohol
(I
f(
Isobutyl Alcohol
it
i€
It
U
((
Isoamyl Alcohol
u
«
Capryl Alcohol
it
AUy Alcohol
Gms.C0(NH^t
t*. per xoo Gms.
Solvent.
194 5.76
20 6. 17
81 23.46
o 1. 01
19 1.65
41 3- 12
60 4.40
80 6.34
98 10
20 I . 18
60 3.41
80 4.88
83 5.24
98 6.15
19.4 0.56
98 2
19.4 9-37
Solubility of Urea in Ethyl Acetate containing Small Amounts
OF Water at 25®.
(Lewis and Burrows, 1911.)
Gms. HiOper 100
Gms. Sorvent.
(Ethyl AceUte+H^).
O
0.652
1. 112
1.638
Gms. Urea
per xoo Gms.
Sat. Sol.
0.080
0.148
0.198
0.296
Gms. H^ per
xoo Gms. Solvent.
(Ethyl AceUte+HiO).
1.677
2.006
2.138
3 234
Gms. Urea
per too Gms.
Sat. Sol.
0.308
0.328*
0.342
o-343t
* A second liquid phaa^ was suspected here*
t A second liquid phase could be dlitlnguished.
UBSA 738
SOLUBILITT OF UrEA IN EtHYL EtHBR.
(Gofftner, 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 S^* 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^. (Dchn, 1917.)
100 gms. aq. 50% pyridine dissolve 21.53 S^s. urea at 20-25^
Diphenyl UBIA.
100 gms. H^ dissolve 0.015 K<n* 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°. (Defan, 19x7)
II
ThioUBSA NHs.CS.NH|.
100 gms. HtO 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, x9x7*)
II
II
AUyl ThioUBSA (Thiosinamine) NHs.CS.NH.C,H».
100 cc. H^ dissolve about 5.9 gms. NHi.CS.NH.CjH* at 15-20®.
100 cc. 90% alcohol dissolve about 50 gms. NHs.CS.NH.CtHi at I5-20^
(Squixc and Cainm, X90S.)
Phenyl ThioUBSA (Phenyl thiocarbamide) CS.NHs.NHCeHt.
Solubility in Water.
(Rothmund, 1900; Biltz, 1903; HoUnun and Antusch, 1894; Bogdan, 1902-03.)
One liter aq. solution contains 2.12 gms. CS(NHs).NHCeH« at 20® (B.), (R.)
and 24 gms. at 25^ (H. and A.). Bogdan gives 2.547 gms. at 25^
Solubility op Phenyl Thiourea at 25® in Aqueous Solutions of.
Potassium Nitrate
.
Sodium Nitrate.
(Bogdan, 1903-03.)
(Bogdan, 1901-03.)
Gms. Mols.
Gms. per
Gms. Mols.
Gms.;
pw -
KNOsper
1000 Gms. HsO.
NaNOs per
1000 Gms.
HtO.
1000 Gms. HiO.
1000 Gms.
HsO.
KNCb.
CS(NHi)
J>ni(feHs.
NaNCb.
^?.«f^
I.04S
105.7
2.38
1.024
87.14
2.26
o.S"3
51.84
2.48
0.506s
43.10
2.46
0 . 2026
20.50
2.54
0.2031
17.28
2-51
0.1007
10.19
2.56
0.0986
8-39
2-53
0 .0503
509
2-55
0.0540
459
2.54
0.0333
3-3^
^ss
0-033S
2.84
a '54
Solubility
SBh SohitioiL
NH,NO,
i(NHJ,SO,
PaC],
iBa(NO,),
CsNO,
LiNO,
iMgSO,
KCjHjO,
KBr
KCIO,
KCl
Kl
KNO,
KNO,
RbNO,
iNa,CO,
NaClO,
NaClO^
NaCl
Nal
NaNO,
NaNOj
JNajSO^
739 Phenyl ThioUREA
OF Phenyl Thioukba in Aqueous Salt Solutions at 2o^
(Bilt£, 2903; Rothmund, 1900.)
MHIimob and the Equivalent Cms. CS(NHi)NHCA Dissolved per Liter of
Aqueous Salt Stdution of Concentration:
O.X2S Normal
Millimnh.
12
14
13
13
13
14
13
13
13
13
13
13
14
13
14
13
14
13
13
14
13
13
13
14
13
95
17
SI
12
98
53
96
40
40
50
86
40
12
89
S3
*s
32
29
75
IS
28
98
94
34
19
Gms*
1.97
215
2.05
1.99
2.13
2.21
2.13
2.04
2.04
2.05
2. II
2.04
2.12
2.21
2.03
2.16
2.04
2.09
2.02
213
2.12
2.18
2.00
0.35 Normal
Miffimnla
82
4
84
92
98
90
96
78
95
35
60
73
48
85
65
49
44
52
65
05
83
07
77
82
35
I
2
2
2
I
I
2
Gms*
1.96
2.21
1.96
97
13
27
13
95
97
04
2.06
1.94
2.21
2. II
2.23
1 .91
2.19
1. 91
2.08
2.14
1-95
2.14
2.10
2. II
1.87
0.5 Nomud.
Millimoh
a .03
4.53
1.78
2.22
3-90
5
3
23
93
1-54
2.14
2.80
3.12
2.19
431
3 52
380
I. II
4-39
1.05
3 07
3 58
1.90
4.29
3 32
3.06
0.85
Gms*
1.83
2.22
1.79
1.86
2.12
2-33
2.12
I -75
1.85
1-95
1.99
1.85
2.18
2.05
2. II
1.69
2.18
1.68
1.98
2.06
1. 81
2.18
2.04
1.98
1.63
X Normal
Millimnls. Gms.
10.69 1. 61
14.91 2.27
9.98 1.52
10.44 1-59
13-73
9-43
10.74
11.76
• • •
10.54
14.60
12.82
12.51
8.73
14.22
8.58
12.21
12.56
10.02
13.96
12.57
II .52
8.30
2.10
•43
.62
•79
.60
•23
.96
.92
•33
•17
•32
.86
.92
•52
•13
•92
•75
.27
Solubility of Phenyl Thiourea in Ethyl Alcohol Solutions of
Several Salts at 28"".
Salt.
None
LiCl
a
ct
u
CaQ.
II
U
it
Nonnalky
of Salt
in
QHiOH.
(pure CAOH)
0.168
0.337
' 0.673
1.346
0.061
0.122
0.244
0.487
0.975
(Thorin, 19x5.)
Mols.
NI]^CS.NHCA
per 100 Gms.
Sat. Sol.
0.2065
0.2274
0.2360
0.2440
0.2494
0.2I0I
0.2135
0.2194
0.2279
0.2372
Salt
Nal
«
((
it
it
NaBr
it
a
it
Normality
of Salt
in
QHiOH.
0.043
0.086
0.172
0.343
0.685
0.022
0.043
0.086
0.172
Mols.
NH^.CS.NH.C|H|
per xoo Gms.
Sat Sol.
0.2102
0.2148
0.2198
0.2271
0.2359
0.2098
0.2194
0.2165
0.2257
Phenyl
740
S(H.UBILITY OF PhBNYL THIOUREA IN MIXTURES OF EtHIHL AlCOH0I«
AND Water
AT 25**.
VoL
Bercent
Scohal.
Gnu.
CS(NH|)
NHCtHs
per 100 Gms.
Solvent.
Sp. Gr.
of
Solationi.
Vol.
percent
Aloshol.
Gms.
CS<NHO
NHC^Hb
per ICO Gnu.
Solvent.
Sp.Gr.
of
Solutions.
TOO
95
3-59
4-44
. a •
0.8200
6s
60
3-40
2.80
0.9018
0.9128
90
85
80
75
4.69
4.99
4-70
4-45
0.8389
0.8544
0.8679
0.8810
SO
40
as
15
1.87
I-I3
0.56
0.38
0.9317
0.9486
09679
0.9788
70
3 92
0.8915
0
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**.
(Bogdui, 1902-03.)
In Aq. Propyl Alcohol.
In Aq. Ethyl AlcohoL
G. Mob. Gms. per xooo
Gms. H2O
G. Mols.
CfHsOHper
xooo Gms.
HsO.
Gms. per xooo
Gms.HiO
C1H7OH pel '
xooo Gms. CsHtOH.
H,0.
CsHfOH.
CS(NH^
NHCsHs.
Z.035 62.10
0-5448 32.688
0.1059 6.354
0.05526 3.316
0.04854 2.912
3 587
3-124
2.643
2.599
2.586
I . lOIO
0-5355
0 . 1094
0 .05018
0.03271
49.60
24.12
4-932
2.26
1-473
3-193
2-931
2.629
2.589
2-577
In Propyl Alcohol
ato°.
1. 000 60.06
1. 21
o.ioo 6.01
1.047
Solubility
of Phenyl Thiourea in Aqueous Solutions of Acbtonb,
Mannitol, Cane Sugar, Dextrose, and Urea.
(Bogdan, 1903-03.)
Aqoeaas
KonJEkctTo-
t».
Gms. per xooo Gms.
H^
Aqueous
Non Electro-
lyte.
t\
Gms. per xooo Gms.
H,0.
lyte.
Kon Elec-
CSfNHi)
NH.CoHf.
Kon Elec-
CS(NHi]
trolyte.
trolyte.
NHCsm
(CH.),CO
25
7.478
2.667
CeH„0.
25
180. 40
3.042
((
2.513
2-579
«
90.46
2.83
((
1.908
2-573
«
29.29
2.69
C,H,(OH),
182. II
3 04
11
18.01
2.654
((
91.05
2.78
tt
9-554
2.603
Vu**a^ii
25
3386
3-457
CO(NH,),
63.08
3 306
u
170.4
3 015
U
29 -93
2.893
it
34-36
2.634
tt
6.132
2.618
u
18.28
2-596
tt
4-942
2.605
H
10.09
2.572
tt
2.009
2.572
H
0
342.18
Z.420
tt
0
60.11
1. 310
U
U
34-22
1.044
«
tt
6.01
1.048
741
UBEIDE
UBEIDE OF GLUCOSE CHiOH.(CHOH)4.CH : N.CO.NH..
lOO
nns. 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) NHs.COs.CtHf. (See also p. 296.}
Solubility of Urbthan in Several Solvents.
(Speyen, 1902.)
Interpolated and calculated from the original results which are given in terms
of molecules urethan per 100 mob. solvent.
o
10
IS
20
30
40
o
10
15
20
25
30
40
o
10
15
20
25
30
40
Solubility in Water.
Wt. oi
X cc.
Solu-
tioo.
1.023
I 033
1.042
1 .060
I 073
1.078
1.065
Mds.
COCNHa)
OCA per
xoo Mois.
H3O.
3.61
6.0
15 o
31.0
50.0
65.0
77.0
Gins
CO(NHj)
OCsHaper
100 Gms.
HsO.
17.8
29.7
74.2
153-3
247 -3
321 -4
380.7
Solubility in Ethyl Alcohol.
Wt.of
z cc.
Solu-
tion.
0.8914
0.930
0.950
0968
0.985
I .001
I 035
Mob.
CO(NHa)
OC\H«per
xoo M(MS.
CaH^OH.
23.91
36.0
43 o
50.0
59 o
70.0
88.0
Gms.
COCNH^
OCsHsper
xoo Gms.
CsHtOH;
46.26
69.6
89.2
96.7
114. 1
135-4
170.2
Solubility in Chloroform.
Wt.of
z cc.
Sdu-
tioQ.
Z.404
1.340
1. 310
1.280
1.240
1.203
1. 125
Mds.
CO(NHa)
OC^por
xoo Mols.
CHCls.
27.56
41
46
53
60
67
80
Gms.
CO(NHa)
OCiHsPer
zoo Gms.
CHOs.
20.6
30.6
34-4
39^
44.8
50.0
59-7
Solubility in Methyl Alcohol.
r
Wt.of
z cc.
Solu-
tion.
0956
0.977
0.^89
1. 000
I 013
1.024
1. 045
Mols.
CO(NH,)
OCs^Hsper
xoo Mous.
CH«OH.
31 18
41 .0
47 5
54.5
62.5
72 0
89.0
Gms.
COQNBj)
OCtHtper
xoo Gms.
CH«OH.
86.76
114. 1
132. 1
151-7
173 -9
200.3
247 -7
Solubility in Propyl Alcohol.
Wt.of
z cc.
Solu-
tion.
0.880
0.906
0.923
0942
0.963
0.983
1.025
Mols.
COQm^
OCsHsper
xoo Mols.
CsHrOH.
19.48
31.0
40.0
51.0
60. 0
68.0
85.0
Gms.
COO^a)
OCsUsper
zoo Gms.
CsHtOH.
28.9
46.0
59-3
75-7
89.0
100.9
126. 1
Solubility in Toluene.
Wt.of
z cc.
Sdu-
tioo.
0.887
0.874
0.875
0.883
0.902
0.927
0-995
Mols.
CO(NHa)
OCaHsPer
zoo Mols.
CeHsCHs.
1.77
50
10. 0
16.0
25.0
44.0
85.0
Gms.
CO(NHa)
OCsH per
zoo Gms.
QHsCHs.
1. 71
4.84
9.68
15.48
24.18
42.58
82.24
100 gms. sat. solution in liquid COi contain 4 gps. urethan at the critical tem-
perature, 23.5**; at 30.5® the mixture separates with two layers. (Bttchncr, Z90S-06.)
100 gms. pyridine dissolve 21.32 gms. urethan at 20-25**.
100 gms. aq. 50% pyridine dissolve loi.i gms. urethan at 20-25^
(Dehn, zgz?*)
M
f.
Gms. Cmpd.
periooGms.
• • •
0.526
»ld
0.143
20
0.040
30
0.032
0.008
i • ■
0.021
30
0.410
30
0.041
URETHAN 743
S(H.UBILITT OF UrBTHAN DbRIVATIVBS IN WaTBE.
(Odain. 19x5)
Name. Fonnuk.
Detonal (Diethyl Aceturethan) (CaH|)tCH.CO.NH.CO.OCtHf
Epional (Ethylpropyl Aceturethan) (CiHi)(C|H7)CILCOJ<nLCO.OCiHi c
Dipronal (Dipropyl Aceturethan) (C|Hi)CH.CO.NH.CO.OC|Hi
Probnal (Propylbutyl Aceturethan) (C.Hf)(C«H«)CH.CO.NH.CO.OC|H<
Dibnal (Dibutyl Aceturethan) (C«Ht)iCH.CO.NH.CO.OCsH«
Oenanthyl UietBan CHa(CH,)iCO.NH.CO.OCA
n Isoamyl Uiethan (CiHi)tCH.NH.CO.OC|Hi
a Biomethyl Propyl Aceturea (CiHi)(C|HT)CBr.CO.NH.CO.NBi
Distribution of Urethan Dbrivativbs bbtwbbn Water and Olivb Oil.
Gms. Cmpd. per pigt. Ratio
Name. Foimuk. t*. loo^cc Codc^
ronnuia. ». h^O OUveOa n^T
Layer. Layer. *-™*^*o
Ethyl Urethan NHtCXX>CA ord. 4.52 0.615 0.136(1)
MeUiyl Urethan NHiCOOCHa ord. 7.50 0.275 0.037(1)
Aceturethan CH|CONH.CXX)CA 17-20 2.94 0.389 0.132(2)
Epronal (CiH^(C|H,)CH.COJm.CO.OCA " 0.076 0.257 3.3(2]
Detonal (CA).CH.CO.NH.CO.OQH. " [I'lH l'^^ \-l[l
Veronal (diethylbar- * cO(NHCO).C.(q«). " I'''?? ''•''''' """^^
bituncaad) J ^vFv««xv^^,v,.vv,ia«;t (0.268 0.032 0.12(2)
(z) Baum, 1899; H. von Meyer, 1909. (3) Odaiim, 19x5.
UBIC ACm CiHaNaO,.
Solubility in Watbr.
(Blares and Deniges, 1887; at 15* Magnier, 1875.)
t».
Gms. r»H«N«Oii.
per 100 Gms.
t«.
Gms. CslLJ^40t
per zoo Gins.
t«.
Gms. C|H4N4Qi
per zoo Gms.
HaO.
HjO.
HaO.
0
0.002
30
0.0088
70
0.0305
10
0.0037
40
0.0122
80
00390
IS
0.0053
50
0.0170
90
00498
20
0.006
60
00230
ZOO
0.0625
One liter of very carefully purified COi 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 COs free water dissolves 0.0649 8™- 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, Z909.)
One liter of water dissolves 0.0645 gm. uric acid at 37^. (Bechhold and Ziegler, z9zo.)
One liter of serum dissolves 0.9 gm. uric add at 37^ "
743
UBIC ACID
Sglubility of
Uric Acid in Aqueous Solutions of
(Hift, Jr. and Pftul. xgoo.)
Acid at i8^
Acid.
Ccmoentnition of Aq. Add.
Cms. Uric Add
per 1000 oc
Sat Sd.
Hydrochloric
«
Sulfuric
I
375
6.24
I
3-2
6.4
3-6s
13.69
22.77
4.9
IS -67
31-34
0.0236
. 0.0263
0.037s
0.0227
0.0205
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 H^Oi was prepared by warming to about 120** and allowing to stand.
Portions of the clear solution were diluted with increasing amounts 01 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 m solution calculated by difference. The following results
were obtained.
Wt. % of aq. H»S04 72.5 Jo-S 68 66.5 62.5 59.5
Gms. uric add per zoo gms.
aq. HsS04 6.45 3.85 1.60 0.64 0.35 0.312
An appronmate determination of the solubility of uric acid in alcohol by ex-
traction m a Soxhlet apparatus, gave 0.00008 gms. per 100 cc. A similar determi-
nation with ether as solvent, gjave n^ative results. (Gortner, 19x4.)
100 gms. 95% formic acid dissolve 0.0^ gm. uric acid at 20**. (Asd^ao, 1913.)
pyridine dissolve 0.21 gm. uric acid at 20-2^^. (Dehn, z9x7-)
** aq. 50% pyridine dissolve 0.75 gms. uric acid at 20-25^. "
VALERIC ACm n CHi(CHs)tCOOH (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. CHs(CHi)sCOOH.
100 gms. of the add layer contain 904 gms. CHt(CHt)tCOOH.
/Lieben and Row, 1S71.)
Distribution of Valeric Acid bbtwbbn Bbnzbnb and 95.8% Sulfuric
Acid.
(Gttrwitadi, 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 Add per xoo Gms. Gms. Valeric Add per xoo Gms.
Benzene Layer.
HaSOiUyer.
: Benzene Layer.
HflSOtUyer.
7.60
46.4
I
36.7
4.78
44.8
0.58
3S-2
3.64
43. S
0.29
32.7
2.61
41.4
0.20
30.7
1.62
39. S
0.04
26.1
Z.48
38.1
0.007
a3.8
The coefficient of distribution of isovaleric acid between benzene and water at
room temperature is, cone, in CeHe + cone, in HsO *» 2.744. (King and Narracott. 1909)
VALBSAMIDB8
744
Distribution of Valbramidbs between Water and Olive Oil at 15'
(HanuB, 1903.)
Amide.
Fonnula.
Valeramide
Valerethylamide
Valerdiethylamide
CH,(CH,),CONH,
CH,(CH,)3CONH(CH6)
CH,(CH2)3CON(C2H6)2
Valerdimethylamide CH,(CH2),C0N(CH,),
Lactdiethylamide CH,CH0HC0N(CH6)i
Gms. Cmpd. per
Ratio
per zoo cc.
Conc^
Water GUveOa
Layer. Layer.
Conc.HfO
0.769 0.241
0.313
1.029 0.261
0.254
0.231 1.339
5-797
o.oii 0.379
0.416
1.256 0.194
0.154
(Dehn, 19x7.)
VANIUJN aH,.CHO.OCH,.OH. 1.3.4.
100 gms. HtO dissolve l gm. vanillin at 20-25''.
100 gms. pyridine dissolve 316 gms. vanillin at 20-25''.
Distribution of Vanillin between Water and Ether at 25^.
(Marden, x9i4-)
Gms. Vanillin per loo cc.
HiO Layer. ^
Dist.Coef.
Ether Layer.
0.0164 0.1294 0.108
0.0242 0.1854 O.IIO
0.0403 0.3310 0.104
Fusion-point data for mixtures of vanillin and orthovanillin are given by
Noelting u9io). 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)-
VlBiLTBINX CirHuNOn.
S(H«UBiLiTY IN Several Solvents.
SoNent.
Water
' Water
3% HsBQ, in Aq.
50% Glycerol
Aniline
Pyridine
Piperidine
Diethylamine
Oil of Sesame
VERATBOLE CHiCOCH,),.
F.-pt. data for mixtures of veratrole and P xylene are given by Patemo and
Ampola (1897).
VERONAL (DiethylbarbituricAcid)CO<(NHCO),>C(C,H»),. See also p. 742.
100 cc. HfO dissolve 0.625 8^* 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**. "
r.
Gms. Veratrine
per zoo Gnu.
Solvent.
Authority.
25
0.
057
(u. s. P. vm.)
20
0.
114
rZalai, 19x0.)
ord.
6
*
(Baroni & Barlinetto, xgxx.)
20
37
(Scholtx, 191a.)
20
175
If
20
83
II
20
271
u
20
z.
39
(Aalai, 19x0.)
VESUVIM.
100 gms. watef" dissolve 8.5 gms. vesuvin at 20-25".
" pyridine " il.l
aq. 50% pyridine " 31.4
4<
If
fl
ft
II
II
II
(Defan, X9X7<)
M
M
745 WATER
WATER HtO.
Solubility of Water in Benzene, Pbtrolbum and Paraffins Oil.
(Gnwchuff, Z9ZZ.)
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 oenzene was of om » 0.8799. The petroleum was American
water white, o( d = 0.792. It was freed from HjO 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 200*^-300^ at 10 mm.
pressure.
Results for:
HiO + Benzene. H2O + Petroleum. HiO + Paraffine Oil.
^e Gms. HflO ^o Gms. H|0 ^* Cms. H^ m Gms. H^
' per TOO Gms. Sol. * per xoo Cms. Sol. ' per zoo Gms. Sol. * per zoo Gms. Sol.
+ 3 0.030 — 2 0.0012 59 0.031 +16 0.003
23 0.061 +18 0.005 61 0.03s 50 0.013
40 0.114 23 0.007 66 0.043 ^5 0.022
SS 0.184 30 0.008 79 0.063 73 0.030
66 0.255 36 0.012 85 0.075 77 0-035
77 0-337 S3 0026 94 0.097 94 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, zQo^zo.)
The results are in terms of the coef . of absorption fi, as defined by Bunsen (see
p. 227) and modified by Kuenen in respect to the substitution of mass for volume
of water.
t*. o*. zo*. so*. 30*. 40*. so*.
Abs. Coef . j3 0.2180 0.1500 0.1109 0.0900 0.0812 0.0878.
NitroZYLENES.
100 gms. 95% formic acid dissolve 0.71 gm. trinitro-m-xylene (m. pt. 173®) at
I8^5 • (Aachan, Z913.)
F.-pt. data for mixtures of 2.3, dinitro-^xylene and 2.6, dinitro-^xylene are
given by Blanksma (1913).
ZTLENOL 1.3.4, C«H,.(CH,),.OH.
MisciBiLiTY OF Aqueous Alkaline Solutions of Xylenol with Several
Organic Compounds, Insoluble in Water.
(Slieuble, Z907.)
To 5 cc. portions of aa. 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.
r' A ■ ■ ^
cc. Aq. KOH. cc. Aq. Insol. Cmpd. Gms. Xylenol.
5 2 (= 1.64 gms.) Octyl Alcohol (i) i
5 5 (=4.10 " ) " 1.7
5 2 (=1.74 " ) Toluene 4.1
5 - 3 (=2.61 « ) " 5
(z) Tbe nonnal secondozy octyl alcohol, s.«., the so-called capzyl aloohd, CH«(CH|)|.CH(0H)CH|.
TTTIBBIUM 746
CobaltiCYANIDE Ybi(CoC«N«)s.9HiO.
1000 gms. aqueous 10% HCl (du « 1.05) dissolve 0.38 gm. of the salt at 25^
(Jmma and WiUand, 1916.)
TTTKRBIUM OZALATI Ybs(Ct04)i.ioHtO.
SOLUBILITT IN WaTBR AND IN SSVBRAL AqUBOUS SOLUTIONS.
Aqueous Solution of: Per cent Cone. «• Gns. Yb|(C«Qi)i a..*i.»»j*«
olAq.Sol. ^' pcrioocc^^oRSS. Authority.
Water ... 25 0.000334 (Rimbach and Schubert, 1909.)
(NH4)2Ct04.HsO 3.26 Ord. 0.095 (Cleve, 190a,)
Methylamine Oxalate 20 '' 5 • 24* (Gnnt and jamet, 19x7.)
Ethylamine Oxalate 20 " SS6*
Triethylamine Oxalate 20 " 2.05*
Sulfuric Add (i n) 4.9 ** 0.372 (Oeve. 1909.)
* The authors do not state whether their figures are for anhydrous or hjrdrated salt.
TTTEBBIUM Dimethyl PHOSPHATI Yb,[(CH,)tP04l<.
100 gms. HtO dissolve 1.2 gms. Yb3[(CHt}sP04]s at 25"* and 0.25 gm. at 95^
(Morgan and James, 19x4.)
TTTEBBIUM SULTATB Yb,(SO«)t.8HiO.
Solubility in Water.
(Cleve, 1903.)
t;
Gms. Ybi(SO«)s
per 100 gma.
H|0.
t».
Cms. VWS04)s
per 100 Gms.
UsO.
t«.
Gms. yWSOJs
per ICO Gms.
HjO.
0
iS-5
35
44.2
34.6
19. 1
55
60
70
"•5
10.4
7.22
80
90
100
6.92
5 83
4.67
TTTEBBIUM Bromonitrobenzene SULFONATE Yb(C«HtBr.NOf.SOi, 1.4.3)1.-
12H1O.
100 gms. sat. solution in water contain 7.294 gms. of the anhydrous salt at 25^.
(Kats and James, 1913.)
TTTBIUM CHLOBIDE YCU.
100 gms. alcohol dissolve 61. i gms. YCU at 15**. (Matignon, 1906.)
" " 60.5 gms. YCU at 20**. (Matignon, X909.)
" pyridine dissolve 6.5 gms. YCU at 15**. (Matignon, 1906.)
TTTBIUM CobaltiCYANIDE Y,(CoC«N«),.9HiO.
1000 gms. aq. 10% HCl {dn ■■ 1.05) dissolve 2.78 gms. of the salt at 25**.
(James and Willand, x9x6.)
TTTBIUM GLYCOLATE Y(C,HsO,)t.2HtO.
One liter of water dissolves 2.447 gms. of the salt at 20^.
(Jantsch and GiUnkxaut, 191 3-19x3.)
TTTBIUM lODATE Y(IOt)i.3HiO.
100 gms. HsO dissolve 0.53 gm. yttrium iodate. (Beriin.)
TTTBIUM MALONATE Ys(CtHs04},.8HiO.
Solubility in Aqueous Malonic Acid and Ammonium Malonatb
S(x«utions.
(Holmberg, 1907.)
Gms. Ys(CAOJa
>ums.
Solvent. t*. per zoo
Solvent.
1 Gm. Am. Malonate per 10 cc. Solution 20 0.3
2 Gms. Malonic Add per 10 cc Solution 20 2.3
747 YTTRIUM NITR4TK
YTTRIUM Basic NITR4TI 3YtO1.4NtOs.2HtO.
Equilibrium in the System Yttrium Nitrate, Yttrium Hydroxide
AND Water at 25®. Games and Pratt, 1910.)
The determinations were made with very great care. The mixtures were ro-
tated 4} months.
Gms. per xoo Gms.
Gms. per xoo Gms.
dnot^ ,
nfi.
SoUd Phase.
dnof
Sat Sol.
^'''9' 5nlid rimM_
Sat. Sol. '
Y(N(W.. ^jOjas
Y(N(W.. ?^,.
1.0260
3.13 0.014
Y(OH),
1.4867
73 03 0078 3YA4NA.aH/>
X.I106
13.87 0.034
(1
1.5587
89.06 0.074 "
1. 1907
24.94 0.063
(1
1.6259
103.80 0.075 "
1.2517
33.02 0.160
"+3YA.4NA.aH;iO
I. 6931
122.40 0.080 "
1.3268
44-35 0.114
3YA4N,0nH/)
1.7440
137.10 0.083 " +y(NCWi
I. 4104
58.61 0.095
it
1.7446
141. 6 0 Y(N(Vi
YTTRIUM OZALATI Yt(CA)i.9HtO.
One liter HtO dissolves o.ooi gm. YtCCtO^i at 25^, determined by the elec-
trolytic method. (Rimbach and Schubert, 1909.)
100 gms. aqueous ammonium oxalate solution (3.26% (NH^tCtOi.HtO)
dissolve 0.017 14 gm. Ys(Ct04)i.9HtO at room temp. (Cleve, 1903.)
100 gms. aq. 2.16 n HtSO^ mssolve 0.6884 gm. YtCCtO^t at 25°. (Wirth, 19x3.)
100 gms. aq. 4.32 n HtS04 dissolve 1.4 gms. Yi(Ci04)t at 25^. "
100 cc. aq. 20% methylamine oxalate dissolve 0.877 gm. yttrium oxalate at
ord. temp.
100 cc. aq. 20% ethylamine oxalate dissolve 1.653 gms. yttrium oxalate at ord.
temp.
100 cc. aq. 20% triethylamine oxalate dissolve 1.006 gms. 3rttrium oxalate at
ord. temp. (Giant and James, X917.)
YTTRIUM Potassium OZALATI Yt(Ct04}t4KtCt04.i2HtO.
SOLUBmiTY IN Water at 25®. (Pratt and James, x9xi.)
The determinations were made with great care. The mixtures were constantly
rotated for 8 weeks.
A^ of Cms. per xoo Gms.
Sat. H^-
Sol. Y,(C,04),. KtCO*.
X.008 Trace 1.31
035 0.02 5.30
059 0.06 8.88
096 0.27 14.50
132 0.72 20.27
^of Gms. per xoo Gms.
&t. H^.
SoUd Phase.
Solid Phase.
^' Y,(C,04),. K,C,04.
SoUd Solution
1. 174 1.50 27.44 Y,(Cj04)^4K,C^4.iaHdO
M
I. 199 1.49 32.83
(f
If
X.222 1.48 37.68
t(
M
I. 231 1.42 39.12
K«Ci04
<l
1.228 1.09 38.77
tt
04),.4K,Ci04.Xfl
iH^
I. 218 0 37.87
u
YTTRIUM DimethylPHOSPHATI Yt[(CHs)tP04]6.
100 gms. HjO dissolve 2.8 gms. YtI(CHi)tP04l« at 25** and 0.55 gm. at 95*.
(Morgan and James, 19x4.)
YTTRIUM SULTATI Y,(S04)i.
S(»«UBiLiTY OF Yttrium Sulfate in Aqueous Solutions of Sodium
Sulfate at 25**. Games and Hdden, X9X3.)
Equilibrium was reached very slowly and it was necessary to rotate the mixtures
for 14 months before final equilibrium was reached.
» Gms.
Solid Phase.
Y,(S0«)|.Na«SO4.3Hd0
Gms. per xoo Gms.
Gms. per xoo Gms.
Bfi.
Solid Phase.
4
H|0.
Y,(S04),.
NajSO*.
Y,(S04),. Na,S04.
5. 61
1.29
Y,(S04),
1.90 14.89
6.38
385
((
1.79 16.51
7.40
6.21
It
1.86 18.44
8.43
8.53
" +Y,(S04),JJa,SO«.aHdO
2.99 19.96
5.86
7.57
Yt(SO«)|.Na,SO|.flH,0
3.04 21.05
4.75
7.72
tt
2.27 27.14
342
10.14
M
1.52 28.22
2.36
11.36
M
1. 61 28. 13
2.02
13-42
M
5.38 0
Na«SO,
.xoH^
TTTBIUM SULFONATES 748
Solubility of Yttrium Sulfonates in Water.
Gins.Anliy.
Sulibiutte. Formiik. f. ^^^ Authority.
Gms. H|0.
Yttrium Benzene Sulfonate Y(C|H«S0^t.9Hi0 15 60.4 (Holmbeig, 1907.)
" " m Nitro-
benzene Sulfonate Y(C|Htll0i.SQ^|.7Hi0 15 48.3
Yttrium Biomonitiobenzene
Sulfonate Y(CABrJfQi.S0k.i4.3)i.xoH^ 25 3.88 (KAtzAJames/zj.)
YTTIUUM TAKTBATI Y,(C4H40i}t.5H,0.
Solubility in Aqueous Tartaric Acid and Ammonium Tartrate
Solutions at 20^. (HolmboK, 1907.)
Gnu. Gms.
A-lSo^-t- ^^Set. A,. Sclent. ^^^
Sftt.SQl. Sat. Sol.
1 gm. Am. Tartrate per zo cc. 2 gms. Tartaric Add per 10 cc.
solution 0.6 solution o.oa
2 gms. Am. Tartrate per 10 cc x . i 4 gms. Tartaric Add per 10 cc.
solution solution 0.02
ZEIN (Protein from Com).
Solubility in Aqueous Alcohol Solutions at 25*.
(Gakotti 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. % CiH^H' Gms. Zdn per Vol. % CAOH Gma. Zdn per
in Solvent. 100 Gms. Sat. SoL in Solvent. zoo Gms. Sat. SoL
lo 0.05 60 18.57
20 o.ii 70 19.87
30 0.21 80 7.81
40 0.51 90 4.51
50 1.43 100 0.02
Similar results are given for the solubility of zein in mixtures of CtHiOH + HsO
+ CHCU at 20** and CjHjOH + HiO + acetone at 25".
ZINC ACETATI Zn(CsH«0,},.2HtO.
Solubility in Aqueous Ethyl Alcohol at 25®. (Seidell, 1910.)
mr* or ' Gms. Zn- wr^ or Gms. Zn^
cw^h ^^ (C,HA)i.3H,0 ci'fVU ^^ (CAQi)i?H^
In^lSSt Sat. Sol. per 100 Gms. ,%r«£nf SaLSol. pSnfo^GmT
Insolvent. ^t. Sd. in Solvent. "sat. SoL
o 1. 168 30.80 60 0.920 10.60
lo 1. 127 27.20 70 0.880 7.80
20 1.090 23.70 80 0.850 5.50
30 I 055 20.40 90 0.830 4.20
40 I. 015 17 95 0.825 4
50 0.970 13.80 100 0.796 I. 18*
* -• gms. anhydrous salt. The solid phase was Zn(C|H^f3HfO in all cases except this solution.
100 gms. HsO dissolve 41.6 gms. Zn(CtHsOi)2.HtO at 15**, d of sat. sol. « 1.165.
(Greenish and Smith, 190a.)
100 cc. anhydrous hydrazine dissolve 4 gms. zinc acetate with separation of a
white suspension at ordinary temperature. (Welsh and Broderson, xgxs.)
ZmC ABSENATI Zn,(As04)s.8HiO.
100 gms. 95% formic acid dissolve 0.26 gm. Zni(As04)t at 21^ (Aschan, 19x3.)
ZmC AKSENITE Zns(AsOs)s.
100 gms. 95% formic acid dissolve 0.36 gm. Zni(AsOi)i at 21^. (Aschan, 19x3.)
749
ZINC BENZOATE
ZmC BENZOATI Zn(C7HiOi)t.
SOLUBILITT IN WaTBR.
(Pajetta, 1906.)
t*. IS.9*. X7*.
Gms. Zn(C7H602)i per
100 gms. aq. solution 2 . 55 3 .49 2 .41 2 .05
a7.8». 3i^'. 37.S'. 49.8*. 59.'
1.87 1.62 1.45
ZmC BROMIDE ZnBri.2HsO.
SOLUBILITT IN WaTER.
(Dietz, 1900; see also Etard, 1894.)
-IS
— 10
- s
- 8
o
+ 13
18
Gms. ZnBn Mob. ZoBrs
per xoo Gms. per zoo
Solutiaa. Mols. H3O.
77 13
78-45
80.64
79.06
79-55
80.76
81.46
27.0
29.1
33-3
30.2
3I-I
33-5
35-1
Solid
Phase.
ZnBrs.3HsO
It
ZiiBrs.aH|0
Gms. ZiiBta Mols. ZaBr^
per xoo Gms. per xoo
Solution. MolsiliO.
25
30
37
35
40
60
80
100
82.46
84.08
86.20
85-45
85-53
86.08
86.57
87.05
37-6
42.3
50.0
46.9
47-4
49-5
S^'S
53-8
Solid
Phase.
ZiiBrs.aHiO
ZoBxi
ZINC BICARBONATE Zn(HCOi)s.
Solubility of Zinc Bicarbonate in Water Containing Carbon Dioxidb.
(Smith, 1918.)
For description of the experimental method see iron bicarbonate, p. 336.
Atmospheres
Presstireof
CO,, Calc. by
Henry's Law.
4.12
5-33
7.64
10.61
12.16
13.29
19-73
20.65
22.56
40.61
Results at 25"*.
Results at 30®.
Gm. Mols.
FreeHtCQa
per Liter.
0.1390
0.1797
0.2579
0.3580
0.4103
0.4480
0.6657
o . 6969
0.7610
I. 3701
Gm. Mols.
Zn(HC0|)s
per Liter.
0.00194
0.002II
0.00242
0.00270
0.00278
0.00291
0.00317
0.00319
0.00343
0.00445
Gm. Mols.
FreeHflCO^
per Liter.
0.1838
0.3838
0.4038
0.4601
0.6064
0.6257
0.7470
0.8351
1.0840
I. 1275
Gm. Mob.
ZnCHCO^,
per Liter.
0.00215
0.00277
0.00286
0.00308
0.00324
0.00337
0.00352
0.00376
0.00339
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 lo"* gms. mols. per liter." (Smith, 1918.)
ZINC CAKBONATB ZnCOt.
Ageno and Valla (191 1) report that the solubility of ZnCOt in water at 25^ is
1.64.10"^ mols. = 0.206 gm. per liter.
One liter of aq. 5.85% NaCl solution dissolves 0.0586 gm. ZnCOt at 14".
One liter of aq. 7.45% NaCl solution dissolves 0.0477 gm. ZnCOs at 14®.
(Cantoni and Paasamanik, 1905.)
ZmO CHLORATB
750
ZINC CHLORATI ZnClO..
Solubility in Water.
(Meusser, 1902; at x8*, Mylius and Funk, 2897.)
r.
-18
o
8
IS
18
Gma. Mols.
9.70 Zn(aOi)|.6HgO
11.08
H.72
15.96
15.39 Zn(aO,),.4HiO
SduUoa.
55-62
59 19
60.20
67.32
66.52
Gnu. Mds.
^. Zn(C10,}, Zn(Cld)«
per zoo Gma. per zoo Mois.
If
it
Solution.
30 67.66
40 69.06
55 75-44
Ice curve
-1$ 30.27
- 9 26.54
Solid Phase.
.UI9.
16 . 20 ZxkiaO0f4Hfi
17.29
24
i(
u
3-36
2.80
Ice
u
Sp. Gr. of solution saturated at 18^ — 1.916.
ZINC CHLORIDE ZnCl..
Solubility in Water.
(Mylius and Dietx, 1905; see also DieU, 1900; Etard, 1894.)
f X
ms.ZnCl
la per 100 G
ms. Solid
f.^
rms.^nC
i^per 100 G
i2?- Solid
m m ^"
Water.
Solution.
■~ Phase.
Water.
Solution.
^ Phase.
- s
14
"3
loe
9
360
78.3
aiHiO + .HaO
-10
25
20.0
u
6
38s
79-4
ZnQ,.3iHjO
-40
83
45-3
tt
6
298
74.9
Znaa.iiH«0
-62
104
51.0
loc + Znaa^HaO
10
330
76,8
•<
-50
"3
53 0
ZnClawiHsO
20
368
78.6
tl
-40
127
55-9
M
26
423
80.9
.ziHsO+ZnOaasO
-30
160
61.5
^H,0 + .3H,0
26.3
433
81.2
•xiHsO + Znda
-10
189
65-4
ZaCla.3H«0
0
342
77-4
ZnCIaiUO
0
208
67-5
M
10
364
78.4
•1
+ 5
230
69.7
U
20
396
79.8
««
6.5
252.
4 71-6
•«
28
436
81.3
Znaa.HaO + ZnOi
5
282
73-8
tl
31
477
82.7
Znds-HaO -
0
309
75 5
jH,0 + .1 JHsO
25
432
81.2
ZnOfl
0
23s
70.1
Znaa.aiHaO
40
452
81.9
M
6-5
252
71.6
.aiHaO + .3HSO
60
488
83.0
M
10
272
73 I
ZnCb.alH|0
80
543
84.4
U
"S
303
75-2
M
100
61S
86.0
M
"5
335
77-0
.aiHsO + .ziHsO
262
00
100. 0
M
Solubility of Oxychlorides of Zinc in Aqueous Solutions of Zinc
Chloride at Room Temperature.
(Driot, 19x0.)
Gms. per
zoo Gms. HiO.
2nCl,.
ZnO.
8.22
0.0137
23.24
0.138
45-95
0.497
SI. 5
0.604
56.9
0.723
SoUd Phase.
ZnCl|4Ztt0.6H|0
Gms. per zoo Gms. HjO.
«(
i(
tt
tt
ZnCl,.
ZnO.
ooua irnaae.
62.85
0.884
ZnC]|.4Zn0.6H^
96
1-792
(i
124.7
3-213
t(
144.8
2.64
tt
203
1-59
Znat.Zn0.z}HsO
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 Chloridb-Ammonium Chloridb Mixtures in Watbr.
(Meerbuxg, 1903.)
Isotherm for o®.
Isotherm for 20®.
Gmt. per xoo Gms.
Solution.
ZnOa. NH«a:
O 22.8
3-5
Isotherm for 30®.
SoUd
Phase.
NHaQ
Gms. per xoo Gms.
Soltttion.
ZaOa.
0.0
71
10.2
18.0
22.4
24.2
25-7
27s
307
33-9
38.8
42.6
44-3
49
52
SS
59
2
6
4
3
62.1
23.0
23 S
23 -9
24.7
25 -3
26.0
26.1
26.3
26.4
25-7
25 -3
24.4
24.6
21.3
15 -3
II. 9
10. o
7-5
6.8
NH4a4-«
(•
•(
a + ft
h
S
9
12
15
18
23
26
29
32
35
38
40
41
43
46
53
58
62
66
I
5
7
7
o
5
o
5
3
8
7
2
9
2
9
2
4
7
6
NH4CI.
26.9
27.1
27.4
SoUd
Phnae.
NH«a
«t
Gms. per xoo Gms.
Solution.
5
7
9
27
27
27
29.0
29 -5
28.1
27.7
27.0
26.9
26.6
26.3
26.0
21 .0
14-5
11. 1
8.7
7-9
u
NH«Cl+a
It
«(
h
(•
ti
ZnCls.
0.0
9.2
16.0
20.2
24.7
26.3
27.2
30.1
36.8
42.4
43-8
45 o
512
61 .9
66.9
75-6
703
785
76.9
79.8
81.6
NH4C].
29 S
29.4
29.7
30.1
304
30.8
30.2
29.6
28.2
27-3
27 -3
24.4
17.6
10.4
9.2
6.1
7.6
35
1.6
0.0
Solid
Phase.
NHga
«•
NH«a+«
It
u
Znda
a — ZnClfl^NHCla.. h - Znas.aNH«Cl.
100 gms. abs. acetone dissolve 43.5 gms. ZnClt at 18**, du of sat. sol. » 1.14.
(Naumann, 1904.)
100 gms. glycerol dissolve 50 gms. ZnClt at 15.5^. (Ossendowski. 1907.)
100 cc. anhydrous hydrazine dissolve 8 gms. ZnClt at room temp.
(Welsh and Brodeison, 191 5.)
When I gm. of zinc as chloride is dissolved in 100 cc. of aq. 10% HCl and
shaken with 100 cc. of ether» 0.03 per cent of the metal enters the ethereal layer.
(Mylius, X91X.)
ZINC CHROAiATES.
Equilibrium in the System Zinc Oxide, Chromium Trioxide and
Water at 25®.
(GrOger, 19x1.)
An excess of ZnO was, in each case, shaken for 3 days at 25^, with gradually in-
creasing concentrations of chromic acid.
ZnO.
Ci6i. '
Solid Phase.
ZnO.
CxOi.
Solid Phase.
0.409
0.604 4zno.cxol.3Hao
66.1
151
4Zn0.Cx0k^H^
2.24
4.19
ft
83.7
192
" +3Zn0.2CKVHiO
5.86
"5
" +3ZnO.Ci0^.2H,0
123
28s
3ZnO.3CxO^.Hf0
10.7
22.2
37.nO.CxOb.3H^
193
450
<(
26.7
57. S
M
196
461
" +Zn0.Ci0,.H/)
30.4
66.7
" +4ZnO.CiO,.3H,0
202
475
ZnO.CiO^.H«0
32.2
70.6
4ZnO.CxOk-3HfO
389
940
it
ZINC CnmAMATI
752
ZINC CINNAMATE Zn(C.H«CH :CHCOO)s.
100 cc. sat. solution in water contain 0.144 S^i* ^"ic cinnamate at 26.5°.
(De Jong, 1909.)
ZINC CYANIDE Zn(CN)s.
100 cc. concentrated Zn(CsHsOt)t + Aq. dissolve 0.4 gm. Zn(CN)j.
100 cc. concentrated ZnSOi + Aq. dissolve 0.2 gm. (Joannis, 1882.)
100 gms. HtO dissolve 0.24 gm. zinc mercuric thiocyanate, ZnHg(CNS)4 at 15°.
(Robertson, P. W.. 1907.)
ZINC FLUORIDE ZnF,.4HiO.
One liter of water dissolves 16 gms. at 18^.
(Dietz, 1900.)
ZINC HTDBOZIDE Zn(OH)i.
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^. (Bodl&nder, 1898.)
Solubility of Zinc Hydroxide in Aqueous Solutions of:
Ammonia and Ammonia Bases at 17*^-19°.
(Heczp 190a.)
Sodium Hydroxide at Ord. Temp.
(Rubenbauer, 1902 .}
Nonnality
Normality
Gms. ZnO
Gms. per ao cc. Solation
MoL
of
of DU-
peraocc.
Solution.
Dilution of
the Baae.
BolredZn.
Na.
Zn.
the NaOH.
O.0942NH3
O.OOII
0.00185
O.IOI2
0.0040
4 SO
0.236 "
O.OIIO
0.0180
0.1978
0.0150
2.33
0.707 "
0.059
0.0958
0.4278
0.0442
1.06
o.o944NH2CHg
0.0005
0.0008
0.6670
0.1771
0.70
0.472
0.0081
0.0132
0.9660
0.9630
0.48
0.944
0.03
0.0484
1-4951
0.2481
0.31
0.068 NH^CjH,
^ 0.0003
0.0005
a. 9901
0.3700
0.16
0.51
0.0045
0.0074
Moist Zn (OH), used. So-
0.68
0.0098
O.O161
lutions shaken 5
hours.
Solubility of Zinc Hydroxide in Aqueous Solutions of Ammonium
Hydroxide.
Results of Euler (1903).
Results of Bonsdorff (1904) at 25°.
f.
Normality
of Aq.
Ammonia.
Mols. Zn
per Liter.
Normality
of Aq.
Ammonia.
Gms. ZnO
per Liter.
Normality
of Aq.
Ammonia.
Gms. ZnC
per Liter
15-17
0.485
0.013-0. 010*
O.3II
0.85
0.321
0.34
IS-I7
0.97
0.034
0.825
3.84
0.643
0.845
21
0.253
0.0029
1.287
7.28
I. 215
2.70
21
0.259
0.0022*
1.928
S07
21
0.500
0.0097
2.570
7.01
21
0.518
0.0070
3 213
10.16
_ 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)j containing from 55 to 77 per cent HjO were
used and in the two cases marked * ZnO was used.
Bonsdorff used for his second series of determinations, Zn(OH)i precipitated
from the nitrate and brought in moist condition into the ammonia solutions.
753 ZINC HTDBOZIDE
SOLUBILITT OF ZiNC HYDROXIDB IN AqUBOUS POTASSIUM HYDROXIDE
Solutions.
(Kkin, X9za.)
The determinations were made by adding aq. ZnSOi solution (containing one
gm. mol. per liter) to aq. KOH solutions until a permanent precipitate just
appeared. The titrations are also recalculated to mob. per liter and correction
made for the dilution of the KOH solution by the aq. ZnSOi.
Nonnalityof
Aq. KOH.
cc. ZnSOi
Sol. per 50 oc
Aq. KOH.
uicu xaoia. |jcr ijucr 01
I OKIi. 001.
OricConc
KOH.
Corrected Cone,
of KOH.
Cozkc. ofZn.
I
S'S
i
0.9
O.IO
1.78
I3-I
1.78
1.42
0.209
2
2.22
2.5
14.3
17.9
z8.8
2
2.22
2.S
1.56
1.63
1. 81
0.223
0.266
0.272
3
3.6
24.6
29.1
3
3.6
2.02
2.28
0330
0.368
4
6
34
S6(?)
4
6
2.38
2.78
0.405
0.540
Solubility of Zinc Hydroxide in One Per Cent Aqueous Salt
Solutions at i6®-2o®.
(Snyder, 1878.)
The COs free Zn(OH)s dissolved is calculated as milligrams Zn per liter of the
given salt solution. Additional determinations are also given.
Aq. Salt
Soluliaa.
Mgs. Zn per
Aq. Salt Mg9. Zn per
Solution. Liter Solutiaa.
Aq. Salt M(s. Za per
Liter Solutioa.
Solution. liter Sohitun.
NaCl
SI
K^O, 37. s
KjCO, 0
KCl
43
MgSO« 27
NH,C1 95
CaCl,
57-5
KNO, 17.5
NH,NO, 77
MgCl,
6$
Ba(NO^, as
(NHOjSO, 88
BaCI,
38
ZINC lODATE Zn(IO,)i.
100 gms. HsO dissolve 0.87 gm. Zn(IOi)t cold and 1.31 gms. hot.
(Rammelabeis, 1838.)
ZmC IODIDE Znl,.
Solubility in Water.
(Diets, 1900; see also Etaid, 1894.)
Cms. ZqIs Mob. Zola Gms. Zols Mols. Z11I9
t*. per ICO Gms. per xoo Solid Phase, t®. per ico Gms. per zoo Mus. Solid Phase.-
Solution. Mols. HiO. Solutioa. HaO.
— 10 80.50 23.3 ZnIi.aHsO o 81.II 24.2 Znlj
— 5 80.77 23.7 " i8 81.20 24.4
o 81.16 24.3 •• 40 81.66 25.1
+ 10 82.06 25.8 •• 60 82.37 26.4
22 83.12 27.8 •• 80 83.05 27.5
21 89.52 50.3 " TOO 83.62 28.7
Sp. Gr. of sat. solution of the anhydrous salt at 18^ » 2.725.
100 gms. glycerol dissolve 40 gms. Znis at 15.5°. (OasendowskI, 1907.)
ZINC NIT&4TI
754
b*^^# *
■mtk^mm^A^ a
Solubility in Water.
(Funk, 1900.)
Gms.
Molti.
Gms.
Mob.
t:
ZnCSOthvet ZnNO»per
loo Gms. loo
SoUd f.e Zii(N(X)iper
Phax. " * 100 Gnu.
Zn(NOt)s per
100
Solid
Phase.
Solution.
Mols. HsO.
Solution.
Mols. HsO.
-25
40.12
6.36Zn(NO.),.0lWl8
53 50
10.9 Zn(NOt)sj6BbO
— 22.
5 40.75
6.54
25
SS-90
12.0
M
— 20
42.03
6.89
364
63 63
16.7
••
-i8
43-59
7-34
36
64.63
17.4
M
-i8
44 63
7.67 Zn(NOi)|j6H,0 33.5
65-83
18.3
M
-IS
45.26
7.86
37
66.38
18.8 ZD(NQ|),4HflO
-13
45 51
7-94
40
67.42
19.7
M
-12
45-75
8.01
41
68.21
20.4
M
O
48.66
9.01
43
69.26
21.4
«•
+-12.
s 52-0
10.3
45 5
77-77
33-3
«
ZmC OZALATI ZnCtO«.2HiO.
One liter HsO dissolves 0.0057 gm. ZnCs04 at 9.76^, 0.0064 S^. at 17.92^ and
0.00715 gm. at 26. 1 5^ (Kohlnusch, 1908.)
Solubility of Zinc Oxalate in Aqueous Ammonium Oxalate
Solutions at 25®.
(Kunschert, 1904.)
Mol. Normal (NH4)2Cs04 0.05 o.io 0.15 0.20 0.25
Mol. Zn per Liter 0.0022 0.0055 0.01055 0.0174 0.0257
Complex ammonia zinc Oxalates are formed. When more than o. 15 free oxalate
is present the complex has the formula, (NH4)4Zn(Cs04)i. In the more dilute
solutions it has the composition, (NH4)sZn(Cs04)s.
ZINC Ammonium PHOSPHATE ZnNHiPOi.
One liter sat. solution in water contains 0.0136 gm. ZnNH4P04 at 10.5^ and
0.0145 gm. at 17.5*
(Aitmann, X9X5.)
ZINC SULFATE ZnS04.
Solubility in Water.
t*.
Gms. ZnS04
per TOO Gms
Solid
Phase.
Gms. ZnS04
Solution.
per 100 Gms. Solid
Solution.
Water:
•
Water. ?»»«•
- 5
28.21
39 30
ZnS04.7HsO
25
38 -94
63 . 74 ZnS04.6HsO
0.1
29 -54
41 -93
M
39
41.22
70.06 />HsO + .7HaO
9.1
32.01
47 09
M
SO
43-45
76.84 ZnS04^HaO
15
33-81
50.88
W
70
47-5
88.7 J6H,0 + Jla0
25
36.67
57 90
H
80
46.4
86.6 ZnSO«JIiO
35
39 98
66.61
14
90
45-5
837
39
41.21
70.05
M
100
44-7
80.8
- 5
32.00
47 08
ZnS04j6HsO
120
41.7
7I-S
01
33-09
49.48
(1
140
160
38 0
33-0
61 .3
49-3
The Sp. Gr. of a sat . sol. of ZnS04 in water at 1 5^ is i .452. (Greenish and Smith, 1903.)
Data for the solubility of ZnS04 in water at high pressures are given by Cohen
and Sinnige (1909, 1910.)
755
ZINC SULFATK
SoLUBiLrry of Zinc Sulfate — Sodium Sulfate Mixtures in Water.
(Koppd, Gompery, 1905.)
O
5
25
30
35
40
10
IS
20
25
30
35
38
40
10
15
20
25
30
35
40
Gms.
Gms.
SdSOT"
per xoo
Sol
lutioa.
27
27
17
17
17
17
29
30
32
34
36
38
38
38
27
24
19
13
6
S
5
.19
S-
•8s
6.
•S8
15 •
.66
15
•59
^5-
•75
15 •
.16
7-
.70
6.
•51
5^
•36
4-
.28
3-
.18
3-
•83
2.
.26
2.
.91
7-
.28
10.
.14
14 •
•31
19.
.96
27.
.61
30 •
.96
28.
NaaSQi
33
27
63
58
70 •
72
16
40
36
41
80
30
90
78
92
90
58
94
75
03
65
Gms. per zoo
Gms HfO.
ZnSQi.
40
42
26
26
26
26
45
48
52
56
60
65
66
64
43
36
28
19
10
8
9
•30
1-
.28
9-
•32
23-
•47
23-
•36
23 •
.68
23-
•79
II.
.81
10.
•34
8.
•15
1-
•55
6.
•25
S-
.64
A-
.89
4-
•50
12.
.92
16.
•77
21.
•93
29.
.67
42.
.72
46.
.16
43 •
90
52
40
44
52
63
24
17
62
22
34
64
98
71
34
71
95
87
51
61
83
Mols. per xoo
Mols. H2O.
2nS04
450
4.71
2.94 2.96
2.95 2.97
2.94 2.98
2.98 2.99
5. II 1.42
5-45 I 29
5.84 1.09
6.27 0.91
6.76 0.81
7.28 0.71
7.44 0.63
7.24 0.60
4.85 1.565
4.12 2.12
3.21 2.79
2.22 3.785
179 5-39
0.971 5.91
102 s-sss
Solid
Phase.
NaiSQt.
I 01 )ZnS04.7HsO +
j 21 1 NaaSOt.ioHK)
J
ZiiNaa(SO«),^HaO
,ZDNas(SO<
WS^-^
!^2^^^^
+NaiSOt.xoHs0
) ZnNaa(SO«)s4H|0
Solubility of Zinc Sulfate in Aqueous Ethyl Alcohol.
(Schiff, 1861.)
Concentration of Alcohol 10 per cent 20 per cent 40 per cent
Gms. ZnS04.7HsO per 100 Gms. Solution 51 . i 39 3 . 45
100 gms. abs. methyl alcohol dissolve 0.65 gm. ZnS04 at 18**, 5.90 gms.
ZnS04.7H,0 at iS**.
100 gms. 50 per cent methyl alcohol dissolve 15.7 gms. ZnS0.7HiO at 18®.
(de Bruyn, 189a.)
100 gms. glycerol dissolve 35 gms. zinc sulfate at 15.5^. (Ossendowskl, 1907.)
ZINC SULFIDE ZnS.
One liter HiO dissolves 70.6. lO"* mols. ZnS = 0.0069 pn. at 18®, determined
by the conductivity method, assuming complete dissociation and hydrolysis.
(Weigel, 1906, 1907.)
ZmC SULFITB ZnS0s.2H,0.
100 gms. HiO dissolve 0.16 gm. ZnSO|.2HiO. (Houston and Trichborae, Z890O
ZINC SULFONATES
Name.
Solubility in Water.
Fonntila.
Zinc /8 Naphthalene Sulfonate (CioH7.SOs)iZn.6HsO
Zinc 2-Phenanthrene " (Ci4H9.SOi)2Zn.6H20
3- " " (C,4H9.SOi)^n.4H20
10- " ** (Ci4H9.SQa)jZn.6HiO
Gnu. Anhy.
t*. Salt per 100 Authority.
Gms. H3O.
25 0.4s (Witt, 191S.)
20 0.083 (Sandquist/ia.)
20 0.19 "
20 O. IS "
ZINC SULFONATES 756
Solubility of Zinc Phbnolsulfonate, p (CcH4.0H.SOs)iZii.8HiO, in
Aqubous Alcohol Solutions at 25*".
' (Seidell, 19x0.)
o 1.18s 39-8 80 1.057 40-7
20 1. 161 40.7 90 1.047 41 -4
40 I- 139 42.1 92-3 1.048 41.9
47 ••• 42.2 95 1.052 42.9
60 1. 106 41.6 100 I' 075 48.8
100 gms. HiO dissolve 37 gms. (C«H4.0H.SOt)iZii.8HiO at is"* and i» of sat.
sol. = 1. 1 62. (Greenish and Smith, 190a.)
ZINC TABTRATK C4H4Ot.Zn.2HsO.
Solubility in Water.
((^toni and Zachoder, 1905.)
Gms.
On».
Gms.
f.
C«HA-7.n.3H^per
f.
C4H4O1.Zn.3H/) per
f.
QHA.Zn.3H^ per
zoo cc. Solution.
xoo cc. Solution.
100 cc. Solution.
15
0.019
40
0.060
65
• O.IOO
20
0.022
45
0.073
70
0.088
25
0.036
50
0.087
75
0.078
30
0.041
55
O.I16
80
O.OS9
35
0.05s
60
0.104
85
0.041
ZmC VALERATK Zn(C4H',COO)s.2HsO.
Solubility of Zinc Valerate in Aqueous Alcohol Solutions at 25®.
(Seidell, 19x0.)
qHJok
in Solvent.
Gms. Zn(C4Hr
in Solvent.
Gms. Zn(C4Hr
Sat. Sol.
C(X)),.aH/)
per 100 Gms.
Sat. Sol.
iaof
Sat. Sol.
C(X)),.aH^
periooGms.
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
60
0.894
I-I5
95-
0.832
8.80
80
0.848
1.70
100
0.844
15.60
ZmCGNIXTM SULFATE Zr(S04)s.
Solubility of Zirconium Sulfate in Aqueous Sulfuric Acid at 37.5**.
(Hauser, 1907.)
Gms. per zoo Gms. Sat. Sol.
ZrO,.
so*.
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
0.14
46.8
Solid Phase.
Zr(S04)s.4H/)
II
II
II
II
II
II
II
ZiOj.
SO,.
Solid Phase.
0.15
56.7
Zr(S04),.4HaO
0.50
57.5
II
2
59.5
II
4.4
61.4
" +Zr(SO«),.H«SO«.3H/>
4.55
61. s
Zr(S04)s.HtSO«.3H,0
3.33
63.8
M
1.80
64.2
l<
I. 12
66.8
II
0.96
68.4
II
O.IO
81. 5
Zr(SO«),.H|SO«.H^
Results at 22® show only slight differences from the above fip^res, hence, the
temperature coefficient for this salt is cjuite small. In an earlier paper Hauser
(1905) gives data for the basic sulfate 4ZrOs.3SO«.i4HsO.
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 p)oint 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 guch 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
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 E^rl 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 contJLct 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-
toning 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 lai^er 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 lar^e test tube C containii^
the excess of salt and solution. The test tube was immersed in the oil
Fig. 4. F[c. 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 lai^e 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 /. 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 5. 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 S 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 (191 1), 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 (191 1),
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 £, 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 J 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 accompHshed 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 DETERUINATION OF SOLUBUITY
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 vfiih a brass tube K, to which the pulley M is attached, and
Fig. 9.
FiQ. 10.
is also pierced by the tightly cemented-in glass tube 7. The glass
rod G, 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 CC^ in the saturat-
ing vessel is provided by introducing COj under pressure through
I and allowing the excess to escape through the mercury seal in E.
After charing the apparatus, I is closed with a rubber tube and
plug and the stirrers fl' if if set in motion. A Witt stirrer, 0,
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 COi 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 detennination of the solubility of thallium hydroxide
at temperatures up to 40* is shown in Fig. 10, As will be seen, this
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. 11 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: AUyl 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 Af. 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 £, 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 o.oi**. 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 Jrom Undissolved SoUd. — The
next point, after the establishment of equilibrium between the
TiPt/Mt*
Fig. 13.
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 co5rdinate 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 OF 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, frequentiy 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 lo 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 ordef 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, J5, 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, AgB^ 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.
Titration 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
776
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
equilibriuni 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 diflference. 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 = Aoo= /</+/*,
where /« and /* 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 ri by the equation
A = -, in which ri represents the concentration in gram-equivalents
per cubic centimeter. Rearrangement and substitution give
ri = J — 7—r. From this equation the solubility of the substance
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 theOstwald "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. ^4 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
780
lETHODS 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 heal 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 / and J. The differences in temperature between the
pipet and buret were never greater than o.i".
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 + at)."
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
fs 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 Hj + C^ 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 HCl. Electrodes
were provided in this vessel and, by means of conductivity measure-
ments, the point determined at which all of the HCl became satu-
rated with NHj. Since the volume of the H2 + Oj required for this
purpose was known, the partial pressure of the NHs 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, 6. A. and Bray, W. C.
(1909) J.Am.Chem.Soc., 31, 729-763.
Abe, RjTttji.
(191 1) Mem.Coll.Sci.Eng. (Kyoto),
3, 212.
(191 1) J.Tok.Chem.Soc., 32, 980.
(1911-12) Mem.Coll.ScLEng.
(Kyoto), 3» 13.
(1912) J.Tok.Chein.Soc., 33, 1087.
Abegg, R.
(1903) Z.Elektrochem., 9, 550.
Abegg, R. and Cox, A. J.
(1903) Z.physik.Chem., 46, 11.
Abegg, R. and Pick, H.
(1905) Ber., 38, 2573.
(1906) Z.anorg.Chem., SV i.
Abegg, R. and Riesenfeld, H.
(1902) Z.phvsik.Chem., 40, 84.
Abegg, R. and Sherrill, M. S.
Z.Elektrochem., 9, 550.
Abegg, R. and Spencer.
(1905) Z.anore.Chem., 46, 406.
Acree, S. F. and Slagle, E. A.
(1909) Am.Chem.Jour., 42, 135.
Adriani, J. H.
(1900) Z.physik.Chem., 33, 453-476.
Ageno, F. and Valla, E.
(191 1) Atti accad.Lincei, 20, II, 706.
(1912) ist.Ven.[VIIIl, 14, II, 331.
(191 3) Gazz.chim.ital., 43, II, 168.
d'Agostino, E.
(1910) Rend.soc.chim.ital. (Roma), 2,
II, 171.
Aignan, A. and Dugas, B.
(1899) Compt.rend., 129, 643.
Alexejew, Wladimir. (Alezejeff.)
( 1 886) Wied.Ann.Physik., 28, 305, 338.
Allen, B. T. and White, W. P.
(1909) Am.Jour.Sci.[4], 27, i.
Altsdiul.
(1896) Monatsh.Chem., 17, 575.
Alluard.
(1864) Compt.rend., 59, 500.
(1865) Liebig's Ann., 133, 292.
Amadoii, M.
(1912) Atti accad.Lincei, 21, II, 67,
184. 769, 690.
(1912a) Atti accad.Lincei, 21, 1, 467,
667-73. .
(1913) Atti accad.Lincei, 22, I, 453,
609; 22, II, 333.
(1915) Atti accad.Lincei, 24, II, 204.
Ainadori, M. and Becarelli, R.
(1912) Atti accad.Lincei, 2X, II, 698.
Ainadori, M. and Pampanini, 6.
(191 1) Atti accad.Lincei, 20» II, 475,
572.
Aniat,L.
(1887) Compt.rend., X05, 809;
Anderson.
(1888-89) Proc.Roy.Soc.(Edin.), 16,
319.
Andrae.
(1884) J.prakt.Chem. [2], 29, 456.
Andrews, L. W. and Bnde, C.
(1895) Z.physik.Chem., 17, 136.
Anon.
(1903) Bull.soc.pharm. (Bordeaux),
p. 7.
(1904) Pharm.Jour.(Lond.), 72, 77.
^ 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 annuelles " for the French title, Tables annuelles de Constantes et
Donnas Numerique de Chemie, de Physique et de Technologie, 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 191 1 and appeared in 1913; and Vol. 3 contains data
for 1912 and was issued in 1914.
785
AUTHOR INDEX
Anthony, C, O.
(191 6) Bonfort's Wine and Spirit
Circular, Apr. loth.
von Antropoff , A
(1909-10) Proc.Roy.Soc. (London),
A 83, 474-83.
Annstroiigy £L E. and Eyre, J. V.
(1910-11) Proc. Roy .Soc. (London),
(A), 84, 12^-135.
(1913) Proc. Roy.Soc. (London), (A),
88,234.
Annstrong, H. B., Eyre, T. V., Hussey,
A. v., and Paddison, w. P.
(1907) Proc.Roy.Soc. (London), (A),
79. 564-576.
Ange, see Ai]g6.
d'Ans, see D'Ans.
d'Anseime.
(1903) Bull.90C.chim. I3], 29, 372.
Archibald, E. H., Wilcox, W. 6. and
Buckley, B. 6.
(1908) J.Am.Chem.Soc., 30, 747-60.
Arctowski, H.
(1894) Z.anorg.Chem., 6, 267, 404.
(1895) Compt.rend., X2X, 123.
(1895-6) Z.anorg.Chem., 11, 272-4.
Armit, H. W.
(1907) Jour.Hygiene, 7, 525-51.
Amdt,K.
(1Q07) Ber., 40, 427.
Amdt, K. and Loewenstein, W.
(1909) Z.Elektrochem., 15, 784-90.
Airhenius, S.
(1893) Z.physik.Chem., 11, 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, 11 17.
Asselln, B.
(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,
I1912-13) ^physik.Chem., 81, 268.
^1913) Z.physik.Chem., 83, 443.
,1914) Z.physik.Chem., 86, 1-35.
(1914a) Z4)hysik.Chem., 88, 321-379.
Atkins, W. K. G. and Werner, E. A.
(1912) T.Chem.Soc.(Lond.), loi, 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 BarschaU, H.
(1908) Arb.Kais.Gesundheitsamt.,
s ^, ^7» 183-230.
(1908) Chem.Ab8., 2, 1125.
Aug6, E.
(1890) Compt.rend., zxo» 1139.
Bagster. L. S.
(191 1) J.Chem.Soc.(Lond.), 99, 1218.
Bahr, F.
(191 1 ) Z.anorg.Chem., 71, 85.
Bakunin, M. and Angrisani, T.
(1915) Gazz.chim.ital., 45, I, 204.
Ball6, RezsO.
(1910) Z.physilcChem., 72, 439.
Baly.
(1900) PhiLMag. I5I, 49, 517.
Bancroft, W. D.
(1895) Phys. Rev., 3, 31, 122, 193,
205.
Bantfaisch.
(1884) T.prakt.Chem., [2], 29, 54.
Barker, T. V.
(1908) J.Chem.Soc.(Lond.), 93, 15.
Barnes, U. T.
(1900) J.Phys.Chem., 4, 19.
Barnes, H. T. and Scott
(1898) J.Phys.Chem., 2, 542.
Baroni, T. and Barlinetto, V.
(191 1) Giorn.farm.chim., 60, 193.
(191 1) " Tables annuelles," 2, 474.
Barre, M.
(1909) Compt.rend., 148, 1604—6;
149, 292.
(1910) Compt.rend., 150, 1321, 1599;
I5i» 871-3.
(191 1) Ann.chim.phys., {8], 24, 149-
167, 202, 210-223.
(1912) Bull.soc.chim. [4], 11, 646.
BascL
(1901) Dissertation(Berlin), p. 17.
Baidcov, A
(1913) Jour.Russ.Phys.Chem.Soc.,
45, 1608.
(1914) Ann.inst.Electrotechnique
(Petrograd), 11, 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.), iii,
620-A2.
Bassett, H. Jr. and Taylor, H. S.
^1912) J.Chem.Soc.(Lond.), loi, 576.
(19 1 4) J.Chem.Soc.(Lond.), 105,
1926-41.
Bathrick.
(1896) J.Phys.Chem., x, 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, B.
(1909) Bull.soc.chim. [4], 5, 1022.
(1909) Compt.rend., 148, 96.
(1912) Ann.chim.phys. [8], 27, 95-8.
(1912a) Bull.soc.chim. [4], 11, 948.
(1913a) Compt.rend., 156, 317.
(1913b) Ann.chim.phys. [8], 29, 131-
136.
(1913c) Bull.soc.chim. [4], 13, 436.
(1913) Ann.chim.phys., [8], 29, 131.
Baud, £. and Gay, L.
(1910) Compt.rend., X50| 1688.
(191 1) Bull.soc.chim. [4], 9, 119.
Baum, Fritz.
(1899) Archiv. exp.Path.u Pharm.,
42, 1 19-137.
Baume, 6.
(191 1) J.chim.phys., 9, 245.
(1914) J.chimjphys., 12, 216.
Baume, (7. and Borowski, W.
(1914) J.chim.phys., X2, 276-81.
Baume, O. and 6eorgitses, N.
(1912) Compt.rend., 154, 650.
(1914) J.chim.phys., 12, 250.
Baume, (7. and 6ennann, F. O.
(1911) Compt.rend., 153, 569.
( 1 914) J.chim.phys., 12, 242.
Baume, 6. and Pamfil, G. P.
(191 1) Compt.rend., 732, 1095.
(1914) J.chim.phys., X2, 256.
Baume, G. and Perrot, F. L.
(191 1) Compt.rend., 152, 1763-5.
(1914) J.chimphys., 12, 225.
Baume, G. and Tykodner, 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.
Bediold and Ziegler.
(1910) Z.angew.Chem., 23, 29.
Beck, K.
(1904) Z.physik.Chem., 48, 657.
Bedc, K. and Stegmiiller, Ph.
(1910) Arb.Kais.Gesundheitsamt.,
34, 447.
(191 1) Z.Elektrochem., 17, 843-48.
Bedanann, £. and Stock, A.
(1895) Z.physik.Chem., 17, 130.
Behrend, R.
(1892) Z.physik.Chem., xo, 265.
(1893) Z.physik.Chem., xi, 466.
Bell.
(1867) Chem.News., x6, 69.
Bell, J. M.
(1905) J. Phys. Chem., 9, 544.
(191 1 ) 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., 11, 637-8.
(1908) J.Phys.Chem., X2, 174.
Bellucd, 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., ^. 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^hysik.Chem., 72, 338-61.
Berju and Kosmsniko.
(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.
(191 1) Proc.Roy.Soc., 85, 503.
Bemardis. G. B.
(1912) Atti accad.Lincei [5], 2X, II,
442.
Bemfeld.
(1898) Z.physik.Chem., 25, 72.
Bertheaume, J.
(1910) Compt.rend., X50, 1064.
Berthelot, M.
(1904) Ann.chim.phys. [8], 3, 146.
(IQ04) Compt.rend., 138, 1649.
Berthelot, M. and Jungfleisch.
(1872) Ann.chim.phys. [4], 26, 400.
Bertrand.
(1868) Monit.Scient. [3J, 10, 477.
Beurafh, A.
(1912-3) J.prakt.Chem. [2], 87, 423.
Bevade, J. (Bewad).
(1884) Ber., 17, K., 406.
(188^) Bull.soc.chim. [2], 43, 123.
Bianchini, G.
(1914) Atti accad.Lincei [5], 23, I,
609.
Bisinem, P.
(1908) Gazz.chim.ital., 38, 1, 559-82.
Billitzer, J.
(1902) Z.physik.Chem., 40, 535.
Blitz, W.
(1903) Z.physik.Chem., 43, 42.
Biltz, W. and Marcus, E.
(191 1) Z.anorg.Chem., 71, 167.
Biltz, W. and mike.
(1906) Z.anorg.Chem., 48, 209.
Birger, Carlson, see Carlson, Burger.
Biron.
(1899) J.Russ.Phys.Chem.Soc., 3X,
517.
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, 924"7«
787
AUTHOR INDEX
BlankBOUL J. J.
(1913) Chem.Weekblad., 10, 136.
(1914) Chem.Weekblad., ix, 28.
Blarez.
(1891) Compt.rend., X12, 434, 939,
1213.
Blarez and Deniges.
(1887) Compt.rend., X04, 1847.
Bodllnder, 6.
(1891) Z.physik.Chem., 7, 317, 361.
(1892) Z.physik.Chem., 9, 734.
(1898) Z.physik.Chem., 27, 66.
Bodllnder, G. and Eberlein, W.
(1903) Ber.. 36, 3948.
Bodlflnder, G. and Fittig, R.
(1901-02) Z.physik.Chem., 39, 597-
612.
BodlXnder. G. and Storbeck.
(1902) Z.anorg.Chem.f 3X, 22, 460.
Bttdtker, B.
(1897) Z.physik.Chem., 22, 510, 570.
Boeke, H. E.
J1907) Z.anorg.Chem., 50, 335.
^191 1 j N.Jahr.Min., x, 48, 61.
,1911) Sitzber.k.Akad.Wiss. (Berlin),
24, 632-8.
Bdeseken, J.
(191 2) Rec.trav.chim., 3X, 354-360.
Bdeseken, J. and Caniere.
(1915) Rec.trav.chim., 34, 181.
B5eseken, J. and Watennan, H.
(191 1) Verslag.k.Akad.Wet.(Amst.),
20, 565.
(1912) Proc.k.Akad.Wet.(Amst.), 14,
620.
Boericke, F.
(1905) Z.Elektrochem., 11, 57.
Bogdan, P.
(1902-3) Ann.Sci.Univ.Jassy, 2, 47.
^1905) Z.Elektrochem., 11, 825.
(1906) Z.Elektrochem., X2, 490.
Bogitch, B.
(1915) Compt.rend., 161, 790-1.
Bogojawlensky, A. and Winogradow,N.
(1907) Z.physik.Chem., 60, 4^3.
(1916) Sitzber.Natur.Ges. Univ. Dor-
pat., xs, 230-37.
Bogojawlensky, A, Winogradow, N.
and Bogolubow.
(1906) Sitzber.Natur.Ges. (Dorpat.),
5.
(1916) Sitzber.Natur.Ges. (Dorpat.),
15, 216-29.
Bogorodsky.
(1894) J.Russ.Phys.Chem.Soc., 26,
209.
(1894) Chem.Centralbl., II, 514.
Bogottsky.
(1905) J.Russ.Phys.Chem.Soc., 37,
92.
Billing.
(1884) Z.anal.Chem., 23, 518.
Bohr, C.
(1899) Wied.Ann.Phy8ik. [3], 68,
503.
(1910) Z.phy8ik.Chem., yx, 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.
Bomwater, J. T. and HoUeman, A. F.
(19 12) Rec.trav.chim., 31, 230.
B<»t>dowski, W. and Bogojawlenski.
(1904) J.Russ.Phys.Chem.Soc., 36,
559-60.
Botta.
(191 1) Zentralbl.Min.Geol., p. 133.
B(5ttger, W.
(1903) Z.physik.Chem., 46, 521-619.
(1906) Z^hysik.Chem., 56, 83-94.
Boubnoff, If. and Guye, Ph. A
(191 1 ) J.chim.phys., 9, 304.
Bougatdt
(1903) J.pharm.chim. [6], x8, 116.
Botdouch, R.
(1902) Compt.rend., X35, 165.
(1906) Compt.rend., 142, 1045.
Bourgoin.
^1874) Bull.soc.chim. [2], 2X, no.
(1878) Ann.chim.phys. [5], X3, 406;
i5» 165.
(1884) Bull.soc.chim. [2], 42, 620.
Boutaric, A
(191 1) 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. [4I, 37, 487.
-Boyle, Mary.
(1909) J.Chem.Soc.(Lond.), 95, 1696.
Boyle, R. W.
(191 1) Phil.Mag. [6J, 22, 840-854.
Bradley. W. P. and Alexander, W. B.
(1912} J.Am.Chem.Soc., 34, 17.
Brainley, A
(1916) J.Chem.Soc.(Lond.), 109,
469-96.
Brand, H.
(191 1) Neues Tahrb.Min.Geol.(Beil.
Bd.), 32, 627-700.
(1912) Zentralbl.Min.Cjeol.and Pal.,
26-32.
(19 1 3) 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.y 54, 569-
608.
Bray, W. C. and Connolly, £. L.
(1910) J.Am.Chem.Soc., 32, 937.
(191 1) 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.
(191 1 ) J.Am.Chem.Soc., 33, 1663.
Breithaupt, J.
( ) Th^, Univ. of Geneve., 38,
No. 446.
Briegleb.
(1856) Liebig's Ann., 97, 95.
Brinton, Paid H. M. P.
(1916) J.Am.Chem.Soc., 38, 2365.
Brissemoret, M.
(1898) J.pharm.chim. [6], 7, 176-8.
Br5nsted, J. N.
^1906) Z.physik.Chem., 55, 377.
(1909) 7th Int. Congress Applied
Chem., 10, no.
(191 1) 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 ZawadsM, J., et al,
(1909) BuU.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, [5I, 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 Gomi, F.
(1899) Atti accad.Lincei, [5], 8, II, 188.
(1900) Atti accad.Lincei, [5], 9, II, 326.
Bruni, G. and Meneghini.
(1909) Z.anorg.Chem., 64, 193.
(1910) Gazz.chim.ital., 40, I, 682.
de Bruyn, C. A. Lobry.
J1890) Rec.trav.chim., 9, 188.
1892) Z.physik.Chem., 10, 782-789.
,1892) Rec.trav.chim., xx, 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, lOI.
. (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.
(19 1 3) Med.K.Vetenskapsakad.No-
belinst, 2, No. 33.
(1913) Chem.Abs., 7, 2886.
Bube, Kurt.
(19 10) Z.anal.Chem., 45, 525-96.
Bilchner, E. H.
(1865) Sitzber.k.Akad.Wiss.(Wein),
52,2,644.
(1905-06) Z.physik.Chem., 54, 665-
88.
BUchner, B. H. and Earsten, B. J.
(1908-9) Proc.k.Akad.Wet.(Amst.),
xx, 504.
Bilchner, E. H. and Prins, Ada.
(1912-13) Z.phys.Chem., 8x, 1 13-120
Bugarszky, S.
(1910) Z.physik.Chem., 7X, 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., x6, 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.
(1912a) Atti accad.Lincei, [5], 2X, II,
72.
Calcagni, G. and Mancini, G.
(1910) Atti accad.Lincei, [5], xp, II,
424.
Calcagni, G. and Marotta, D.
(191 2) Gazz.chim.ital., 42, II, 669-
680.
(1912) Atti accad.Lincei, [5], 2X, II,
93,243,284.
(1913) Gazz.chim.ital., 43, II, 380.
(1913) Atti accad.Lincei, [5I, 22, II,
373. 443.
(i9id) Gazz.chim.ital., 44, I, 487.
Callenaer and Barnes.
(1897) Proc.Roy.Soc., 62, 149.
Calvert, H. T.
(1901) Z.physik.Chem., 38, 521-540,
789
AUTHOR INDEX
CalzoUrifP.
^1912) Gazz.chim.ital., 42, II, 85-92.
( ) Acc.8c.med.e.iiat.dl Ferora,
85f 150.
CambiyL.
(1912) Atti accad.Lincei, [5], 21, I,
776, 791.
(191 2) Atti accad.Liiicei, [5], 21, II,
839.
Cambi, L. mad Speroni^ G.
(191 5) Atti accacLLincei, [5], 24, I,
736.
Cuncfoiif F. K*
(1898) J.Phys.Chem., 2, 413.
(1901) J.Phys.Chem., 5, 556.
Cameron, F. &. and Bell, J. M.
(1905) J.Am.Chem.Soc., 27, 1512.
(1906) J.Am.Chem.Soc., 28, 1220,
1222.
(1906a) J.Phys.Chem., 10, 210.
(1907) J.Phys.Chem., 11, 363.
(1910) J.Am.Chem.Soc., 32, 869.
Cameconi F. K., Bell, J. M., and Robin-
son, W. O.
(1907) J.Phys.Chem., ix, 396-420.
Cameron, F. &. and Breazeale, J. F.
(1903) J.Phys.Chem., 7, 574.
(1904) J.Phys.Chem., 8, 33^.
Cameron, F. K. and Patten, H. E.
(191 1 ) J.Phys.Chem., 15, 67.
Cameron, F. K. and Robinson, W. O.
(1907) J.Phys.Chem., 11, 577, 641,
691.
(1907a) J.Phys.Chem., 11, 273-8.
(1909) J.Phys.Chem., 13, 157, 251.
Cameron, F. K. and SeideU^ A.
(1901) Bull. No. 18, Division of Soils,
U. S. Dept. Agr.
(1901a) J.Phys.Chem., 5, 643.
(1902) J.Phys.Chem., 6, 50.
Campetti, A
(1901) Atti accad.Lincei., [5], xo, II,
99-102.
(1902) Z.physik.Chem., 41, 109,
(abstract).
(19 1 7) Atti accad.sci.Torino, 52,
11^-21.
Campetti, A and Del Grosso. C.
(19 1 3) Nuovo cimento, [6], 6, 379-
417
(1913) Mem.R.accad.Sci. (Torino),
im, 61, 187.
(191 1) " Tables annuelles," 2, 433.
Cantoni, H. and Basadomuu
(1906) Bull.soc.chim., [3], 35, 731.
Cantoni. H. and Diotalevi, D.
(1905) Bull.soc.chim., I3I, 33, 27-36.
Cantoni. H. and Goguelia^ G.
(1905) Bull.soc.chim., [3), 33, 13.
Cantoni. H. and Jolkowdcy.
(1907) Bull.soc.chim. [4], i, 1181.
Cantoni. H. and Passamanik.
(1905) Ann.chim.anal.appl., 10, 258.
Cantoni. H. and Zacfaoder.
(1905) BulLsocchim., [3J, 33, 747.
CapandGarot
(1854) J.pharm.chim., [3], 26, 81.
Capin, J.
(1912) Pharm.Jour.(Lond.), 88, 65,
from (191 1 ) BulLsoc
pharm. (Bordeaux), 414.
CariinfantL B. and Levi-lCalvano, M.
(1909) Gazz.chim.ital., 39, II, 353-
75.
Caxlson^ BiKer.
(1910) Klason-Festschrift, 247-66
(Stockholm).
(1910) " Tables annuelles," x, 379.
Carnelly.
(1873) Liebig's Ann., x66, (xx6.^),
155.
(1873) J.Chem.Soc.(Lond.), [2], 11,
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.(Load.), 105,
1602-11.
Carrara and MinozzL
(1897) Gazz.chim.ital., 27, II, 955.
Cairelli. H. R.
(1898) J.Phys.Chem., 2, 213.
Caspar!, W. A
(1915) J.Chem.Soc.(Lond.), X07,
162-171.
Cassttto. L.
(19 1 3) Nuovo cimento, 6, 1903.
Cavazzi. A.
^1916} Gazz.chim.ital., 46, II, 122-35
(191 7) Gazz.chim.ital., 47, II, 49-63-
Centnerszwer, M.
(1899) Z.physik.Chem., 29, 715.
(1910) Z.physik.Chem., 72, 437.
Centnersrwer, M. and Teletow, L
(1903) Z.Elektrochem., 9, 799.
de Cesaris, P.
(1911) Atti accad.LinGei, [5], 20, I»
597. 749.
Chancel and Parmentier.
(1885) Compt.rend., xoo, 473, 773-
Chandler, B. B.
(1908) J.Am.Chem.Soc., 30, 696.
Chattaway, F. D. and Lambert Wm. J.
(1915) J.Chem.Soc.(Lond.), I07i
1768, 1776.
Chavanne, G. and Vos, J.
(1914) Compt.rend., X58, 1582.
Chilrashigi, M.
(1911-12) Mem. Coll .Sci.Eng. (Kyoto),
3, 197-206.
(191 1 ) Z.anorg.Chem., 7a» 109.
790
AUTHOR INDEX
Chikashisii M. and Yrnnanchi, Y.
(1916) Mem.CoU.Sci.Kyoto, i, 341-7.
Chilesotti, A.
(1908) Atti accadXincei, [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.Chein., 79, 459.
Christyy S. B.
(1901) Elektrochem.Ztschr., 7, 205.
ChugaeT, L. and SIhlopin, W.
(1914) Z.anorg.Chem., 86, 159.
Cingolani, M.
(1908) Gazz.chim.ital., 38, I, 305.
(1908) Atti accad.Lincci., [5], 17, I,
265.
Cittsa, R. and Bernardi, A.
(1910) Gazz.chim.ital., 40, II, 159.
Claasen. H.
(191 1; Z.Ver.Zuckerind.,6x, 489-509.
Cleve.
(1866?) K. Svenska Vetenskaps-
Akad . Handl. (Stockholm) ,
10, 9» 7.
(1874) Bull.soc.chim., [2], 2X, 344.
(1885) Bull.soc.chim., [2], 43, 166.
Cleve, Astrid.
(1902) Z.anorg.Chem., 32, 157.
Cloez.
(1903) Bull.soc.chim. [3], 20, 167.
Clowes, F. and Biggs, J. W. H.
(1904) J.Soc.Chem.Ind., 23, 358.
Cocheret, D. H.
(191 1 ) Dissertation, Leiden.
(191 1) ** 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, B. and Inouje, K.
(1910) Z.physik.Chem., 72, 411-424.
(1910) Chem.Weekblad., 7, 277.
Cohen, B., Inou^e, K. and £uwen, C.
(19 10) Z.physik.Chem., 75, 257.
Cohen, B. and Sinnige, L. R.
(1910) Trans.FaradaySoc., 5, 269.
Cohn, B.
(1895) Z.physik.Chem., x8, 61.
Colani, A.
(1913) Compt.rend., 156. 1075, 1908.
(1916) Bull.soc.chim., (4], 19, 405.
(1916a) Compt.rend., 163. 123-5.
(191 7) Compt.rend., 165, 11 1-3,
234-6.
Colson, A.
(1907) Compt.rend., 145, 1167.
Comanducci, £.
(1912) Rend.soc.chim.ital., [2], 4,
313.
de Coninck, Oechsner.
J1893) 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, 350.
(1906) Compt.rend., Z42, 571.
Conroy.
(1898) J.Soc.Chem.Ind., 17, 104.
Cooper, M. C, Shaw, R. L, and Loooais,
N. E.
(1909) Am.Chem.Jour., 42, 461.
(1909) Ber., 42, 3991.
Copisarow, M.
(191 5) Chem.News., 112, 247.
Coppadoroj A
(1909) Gazz.chim.ital., 39. II, 625.
(191 1) Rend.soc.chim.ital., [2], 3a,
207.
^1912) Gazz.chim.ital., ^2, 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
fi868) Ber., x, 138.
(1869) Z.anal.Chem., 8, 145.
Costachescu, N.
(1910) Ann.Sci.Univ.(Jassy), 7, i.
Coste, J. H.
(191 7) J.Soc.Chem.Ind., 36, 846-53.
(1918) J.Soc.Chem.Ind., 37, 170.
Cottrell. et al.
(1901) Sitzber.k.Akad.Wis8. (Berlin),
p. 1035.
Couch, J. F.
(1917) Am.Jour.Pharm., 89, 243-51.
Courtonne, H.
(1877) Ann.chim.phys., [5], X2, 569.
(1882) Compt.rend., 95, 922.
Cowper, R.
(1882) J.Chem.Soc.(Lond.), 4x, 254.
Creighton, H. J. M., and Ward, W. H.
(1915) J.Am.Chem.Soc., 37, 2333.
Croft
(1842) Phil.Mag., [3], 2X, 356.
Crompton, H. and Walker, M.
(1912) J.Chem.Soc.(Lond.), loi, 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.
Ciino, E.
(1908) Ann.physik., [4], 25, 346-76.
(1908-09) Ann.physik., [4], 28, 663-4.
(1907) Ber.physik.Gcs., 5, 735-8.
Curtis, H. A« and Titus, E. Y.
(191 5) J.Phys.Chem., 19, 740.
Curtius and Jay.
(1889) J.prakt.Chem., [2], 39, 39.
Dahms, A.
(1895) Wied.Aim.Physik.. 54,486-519.
(1896) Wied.Ann.der Physik., 60, 122.
(1899) Ann.chim.phys., [7], 18, 140.
Dakin, H. D., Tanney, N. W. and
Wakemann, A. J.
(191 3) J.Biol.Chem., 14, 241.
▼an Damm, W. and Donk, A. D.
(191 1 ) Chem.Weekblad, 8, 848.
Dancer.
(1862) J.Cheni.Soc.(Lond.), 15, 477.
D'Ans, T.
(1908) Her., 41, 1776-7.
^1909) Z.anorg.Chem., 62, 129-167.
(1909a) Z.anorg.Chem., 63, 225-9.
(1909b) Z.anorg.Chem., 65, 228.
^19090) Z.anorg.Chem., 61, 91-5.
(1913) Z.anorg.Chem., 80, 235.
D'Ans, T. and Fritsche, O.
(1909) Z.anorg.Chem., 65, 231.
D'Ans, J. and ^hreiner, O.
(1910) Z.anorg.Chem., 67, 437.
(1910a) 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.
f 1906) J.Chem.Soc.(Lond.), 89, 1668.
(1908) J.Chem.Soc.(Lond.), 93, 13 10.
(1909) Z.physik.Chem., 69, 1 10-122,
(1909a) J.Chem.Soc.(Lond.), 95,
370-81.
(1909b) J.Chem.Soc.(Lond.), 95,874.
Dawson, U. M. and Gawler, R.
(1902) J.Chem.Soc.(Lond.), 81, 524.
Dawson, H. M. and Goodson, E. E.
(1904) J.Chem.Soc.(Lond.), 65, 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.
(1901a) J.Chem.Soc.(Lond.), 79, 493.
(1901b) J.Chem.Soc.(Lond.), 79,
1069.
Dehn, Wm. M.
O917) J.Am.Chem.Soc., 39, 1400.
(1917a) J.Am.Chem.Soc., 39, 1378.
De Jong (see de Jong).
Delange, Leon.
(1908) Bull.soc.chim., [4], 3, 910-5.
Delepine.
J1892) 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, i860.
Demassieux, N.
(1913) Compt.rend., 156, 892.
(1914) Compt.rend., 158, 183, 702.
Denham, H. G.
(191 7) J.Chem.Soc.(Lond.), iii, 39.
Derick, C. G. and Kamm, O.
(1916) J.Am.Chem.Soc., 38, 415.
Demby, K. G.
(i9i8)Medd.k.Vetenkapsakad.Nobel
inst., 3, No. 18.
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.
(1874) 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.
(1875) Compt.rend., 80, 1164.
(1877) Compt.rend., 85, 1069.
(1881) Compt.rend., 92, 242, 718.
(1881) Ann.chim.phys., [5J, 24, 226.
(1896) Compt.rend., 123, 1282.
(1897) Compt.rend., 124^. jo.
(1898) Ann.chim.phys., [7], 14, 294.
Dittmar.
(1888) J.Soc.Chem.Ind., 7, 730.
792
AUTHOR INDEX
Dittiich. C.
(1899) Z.physik.Chem., 29, 485.
Ditz, M. and Kanhauser, F.
(19 1 6) Z.anorg.Chem., 98, 128-40.
Divers.
(1870) J.Chem.Soc.(Lond.), 23, 171.
(1899) J.Chem.Soc.(Lond.), 75, 86.
Doerinckel, F.
(1907) Metallurde, 8, 201-9, 4^8.
Dolezalek, F. and Finckli, K.
(1906) Z.anorg.Chem., 51, 320-7.
Dolgolenko, W.
(1907) J0ur.Russ.Phys.Chen1.S0c.39,
841.
Dolinski, J. H.
(1905) Ber., 38, 1835.
Donath, £.
(loii) 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.),09, 1788.
Donnan, F. G. and White, A. S.
(191 1 ) J.Chein.Soc.(Lond.), 99, 1669.
van Dorp, G. C. A.
(1910) Z.physik.Chem., 73, 284-289.
^1911) Chem.Weekblad., 8, 269.
(191 2) 8th Internat.Cong.Appl.
Chem., 22, 239.
(1913-14) Z.physik.Chem., 86, 109.
Dott, D. B.
(1906) Pharm.
J1907) Pharm.
^1910) Pharm.^
1 9 12) Pharm.^
our.(Lond.), 76, 345.
our.(Lond.), 78, 79.
our.(Lond.J, 85, 795.
lour.(Lond.;, 88, 424.
Doumer and Deratix.
(1895) J. pharm.chim., [6], i, 50.
Doyer, T. 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, £.
(1910) Z.physik.Chem., 75, 405.
Duboin, A.
(1905) Compt.rend., X41, 385.
Duboin, A.
(1906) Compt.rend., 142, 395, 573,
887, 1338.
Dubois and Pade.
(1885) BuU.soc.chim., [2], 44.
Dubowitz, H.
(191 1 ) Seifensieder Ztg., 38, 11 64,
1208.
( ) Vegnesceti lapok., 6, 397.
Dubrisay, Ren6.
(191 1 ) 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, 327-337;
54.45-9.
(1907) J.Russ.Phy3.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.), loi,
43 1-43-
(1914) J.Chem.Soc.(Lond.), 105,
368-79, 733, 2630.
Dunnington and Long.
(1899) Am.Chem.Jour., 22, 217.
Dunstan, W. R. and XJmney, J. C.
(1892) J.Chem.Soc.(Lond.), 61, 391.
Dupre and Bialas.
(1903) Z.angew.Chem., 16, 55.
Dutilh, H.
(1912) Verh.k.Akad.Wet.(Amst.), [i i)
4,60.
(1912) " Tables annuelles," 3, 336.
Ebelmen.
(1852) Liebig'8.Ann., [3], 5, 189.
Bder.
(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.
(191 2) 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.
Eg^nk, B. G.
(1908) Z.physik.Chem., 64, 492.
Bhlert, H. and Hempel, W.
(191 2) 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.
EnunerUng.
(1869) Liebig's Annafen, 150, 257.
von Ende, C. L.
(1901) Z.anorg.Chem., 26, 148.
EngeL
(1886) Compt.rend., X02, 114.
(1887) Compt.rend., X04. 507, 913.
(1888) Ann.chim.phys., [6], 13, 348-
385.
(1889) Ann.chim.phys., [6J, 17, 347.
(1891) Bull.soc.chim., [3], 6, 17.
Enell.
^1899) Pharm.Centralh., 38, 181.
(1899) Z.anal.Chem., 38, 386.
Engfeldt, N. O.
(19 1 3) Farmaceutisk Revy, No. 8.
(1913) Apoth.Ztg., 28, 182.
(1913) PnarmJour.(Lond.), 90, 769.
Eiu;lisfa^ S. and Turner, W. E. S.
(1915) J.Chem.Soc.(Lond.), 107,
774-83.
EnkUar. J. E.
(190 1) Rec.trav.chim., 20, 183.
EnniSy A. J.
(1914) J.Chem.Soc.(Lond.), 105,
350-^.
Eppel.
(1899) Dissertation, Heidelberg.
Erdmann.
(1893) Ber., 26, 2439.
Erdmann and Bedford.
(1904) Ber., 37, 1 184.
Etard.
(1877) Compt.rend., 84, 1090.
(1884) Compt.rend., 98, 1434.
(1894) Ann.chim.phys., [7], 2, 526-
570; 3» 275.
▼on Elder, H.
;i903) Ber., 36, 2879, 3400-
1904) Z.physik.Chem., 49, 315.
J916) Z.physik.Chem., 97, 291.
▼on Elder, H. and LQwenhamn, B.
(1916) Z.Elektrochem., 22, 199-254.
(1916) Chem.Abs., xo, 3021.
(1917) Chem.Abs., 11, 915.
Euwes, P. C. J.
(1909) Rec.trav.chim., 28, 298.
Ewers, Erich.
(19 10) Milch wirschaft.Zentr., 6 (3?),
155.
▼an Eyk, see Van Eyk.
Fahiion. W.
(1916) Chem.Umschau, 23, Z^S^
FalcioUu 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.f 148, 1189.
(19 10) Ann.chim.phy8., 18], 19, 70-
152.
Fauzer.
(1888) Math.u.Natur.Wiss.Ber.(Un-
garn), 6, i^.
deFazi, R.
(19 1 6) 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.
Felt, w. and Przibylla, K.
(1909) Z.Kali, 3, 393-^.
Fenton, H. T. H.
(1898) T.Chem.Soc.(Lond.), 73, 479.
Fercfalana.
(1902) Z.anorg.Chem., 30, 133.
Field.
(1859) J.Chem.Soc.(Lond.), 11, 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, 121 7.
(1904) J.Chem.Soc.(Lond.), 85, 403.
(1908) Chem. News, 96, 163.
(1908) Analyst. 33, 391.
Findlay, Alex, and Crei^ton. H. J. M.
(1910) J.Chem.Soc.(Lond.), 97, 536—
61.
(191 1 ) Biochemjour., 5, 294.
Findlay, A. and Hickmans, E. M.
(1907) J.Chem.Soc.(Lond.), 9X, 905,
(1909) j.Chem.Soc.(Lond.), 95, 1389.
Findlay. A. and Howell, O. R.
(i9i4)J.Chem.Soc.(Lond.), 105, 291^
98.
(191 5) J.Chem.Soc.(Lond.), X07,
282-4.
Findlay, Alex, and Eling, 6.
ii9^3) J-Chem.Soc.(Lx)nd.), 103,1170.
1914) J.Chem.Soc.(Lond.), 105, 1297.
Findlay, Alex., Morgan, I. and Morris,
LP.
(1914) J.Chem.Soc.(Lond.), X05,
779-82.
Findlay, Alex, and Shen, B.
(1911) J.Chem.Soc.(Lond.), 99) 1 313.
(1912) J.Chem.Soc.(Lond.), lor,
1459-^.
794
AUTHOR INDEX
Findlay, Alex, and WiUiams. T.
(1913) J.Chem.Soc.(Lond.), 103, 636.
Fischer, Emll.
(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.
Flas^hner, O.
(1908) Z.physik.Chein., 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, llby 695-722.
(19 10) Monatsh.Chem., 31, 23-50.
Flawitzki, F.
(1909) J.Russ.Phys.Chem.Soc., 41,
739.
Fliiddger.
(1887) Arch.Pharm., [3], 25, 542.
Fock.
(1897) Z.Kryst.Min., 28, 365, 397.
Fokin, S. J.
(191 2) 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.
(191 2) J.Am.Chem.Soc., 34, 880.
O915) J.Am.Chem.Soc., 37, 290,
1200.
Foote, H. W. and Andrew, L A.
(1905) Am.Chem.Jour., 34, 153, 165.
Foote, H. W. and Chalker, W. C.
(1908) Am.ChemJour., 39, 564, 567.
Foote, H. W. and Haigh, F. L.
(191 1 ) 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, U. W. and Walden, P. T.
(191 1) J.Am.Chem.Soc., 33, 1032.
Forbes, G. S.
(191 1) J.Am.Chem.Soc., 33, 1937.
de Forcrand, R.
(1909) Compt.rend., 149, 719.
(1909a) Compt.rend., 149, 1344.
de Forcrand, R.
(191 1) Compt.rend., 152, 1210.
(1912) Compt.rend., 154, 133.
(1912) Compt.rend., 155, 118, 1767.
de Forcrand, and Fonzes-Diacon.
(1902) Ann.chim.phys., I7I, 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.
(1909a) 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.
(191 2) 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., 11, 258.
Friedel.
(1869) Liebig's Ann., 149, 96.
Friedel and Gorgeu.
(1908) Compt.rend., 127, 590.
Friedel and Lachbui]g.
(1869) Bull.soc.chim., [2], X2, 92.
Friedlflnder, T.
(1901) Z4)hysik.Chem., 38, 389.
Friedrich, K.
(1907) Metallurgie, 4, 480, 671.
(1908) Metallurgie, 5, 114.
(1914) Metallurgie u.Erz., xx, 196-
200.
Ftonmiiller.
(1878) Ber., XI, 92.
795
AUTHOR INDEX
Fujimtirat T.
(1914) Mem.Col.ScLKyoto, x, 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.
(1900a) Ber., 33, 3697.
Fttrcnt, 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, 6.
(1906) Z.physiol.Chem., 48, 473.
Galeotti, C. and Giampalmo, G.
(1908) Z.Chera.Ind.koUoide, 3, 118-
25.
Garelli, 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.
(19 10) Compt.rend., 150, 467.
Gaus.
(1900) Z.anorg.Chem.. 25, 236.
Gav-Lnasac.
(1819) Ann.chim.phys., 11, 314.
Gazarolli and Thumbalk.
(1881) Liebig's Ann., 209, 184.
Geffcken, G.
(1904) Z.physik.Chem.y 49, 271, 296.
Geiger.
(1904) Dissertation (Berlin).
Gemsky, N.
(1914) Neues Tahrb.Min.(^eol.(Beil.
Bd.), 36, 513-58.
▼on Geordevics, G.
(1913) Z.physik.Chem., 84, 358.
(191 3) Monatsh.Chem., 34, 734.
(191 5) Z.physik.Chem., 90, 54.
(19 1 5) Monatsh.Chem., 36, 400.
Gerard.
(1901) rinn.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.
(191 1) Verslag.k.Akad.Wet.(Arast.),
30, 337.
▼an Ginneken, P. J. 'EL
Z.Ver.Zuckerind, 63, 421—39.
Ginsberg, A. S.
(1906) Ann.Inst.Polyt.(Petrograd), 6,
493.
^1908) Z.anorg.Chem., 59, 346.
(1909) Z.anorg.Chem., 61, 122.
Giolitti, F. and Bucd, G.
(1905) Gazz.chim.ital., 35, II, 162-9.
Giolitti, F. and VecchiareUi, V.
(1905) Gazz.chim.ital., 35, II, 170.
Giran, H.
(1903) Jour.physique, I4], 2, 807.
(1903a) Ann.chim.phys., [7], 30, 249.
(1906) Compt.rend., 142, 398.
^1908) Compt.rend., 146, 270, 1270.
(191 3) Bull.soc.chim., [4], 13, 1050.
Giraud, H.
(1885) Bull.soc.chim., [2], 43, 552.
▼on Girsewald, C. and Wolokitin, A.
(1909) Ber.. 42, 856-9.
Giiia, M.
(1914) Ber., 47, 1718-23.
(1915) Gazz.chim.ital., 45, I, 339,
557; n, 32, 348.
(1916) Gazz.chim.ital., 46, 1, 289; II,
274.
(1916) Atti accad.Lincei, [5], 25, I,
99-105.
Gladstone.
(1854) J.Chem.Soc.(Lond.), 6, 11.
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.
Gdckel.
(1897) Chem.Zentralbl., II, 401.
Godeffroy.
fi876) Ber., 9, 1337, 1169.
(1886) Z.Sster.Apoth.Ver., No. 9.
Goldblum, H. and Stoffella, G.
(loio) J.chim.phys.. 8, 154.
Goldblum, H. and Terlikowski, F.
(1912) Bull.soc.chim., [4], xi, 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.
Goldsdunidt, H. and Eckardt, M.
(1006) Z.physik.Chem., 56, 389.
Goldsdunidt H. and Sunde, E.
(1906) Zj)nysik.Chem., 56, 15.
Goodwin, w. L.
(1882) Ber., 15, 3039.
▼an der Goot, Tetta Polak.
(1013) Z.physik.Chem., 84, 419-450.
Gordon, V.
(1895) Z.physik.Chein., z8, 1-16.
796
AUTHOR INDEX
Gore.
(1870) Proc.Roy.Soc., 18, 158.
Gori,G.
(191 3) Boll.chim.farm., 52, 891-5.
(191 5) Chem.Abs., 9, 1827.
Gortner. R. A.
(19 14) Biochem.Bull., 3, 468-9.
Gothe, E.
(1915) Chem.Ztg., 39, 305-7.
Qott, B. S. and Muir, M. P.
(1888) J.Chem.Soc.(Lond.), 53, 138.
Grahmann, W.
(1913) Z.anorg.Chem.y 81, 257-314.
Grant, A. J. and James, C.
(191 7) J.Am.Chem.Soc., 39, 934.
Green, W. F.
(1908) J.Phys.Chem., 12, 655-60.
Greeni^, H. G.
(1900) Pharm.Jour.(Lond.), 65, 190-
95.
Greenish, H. G. and Smith, F. A. XT.
(1901) Pharm.Jour.(Lond.), 66, 774-
777, 806-811.
(1902) Pharm.Jour.(Lond.), 68, 510-
532.
(1903) Pharm. Jour. (Lend.), 71, 881.
Grehant, N.
(1894) Compt.rend., 118, 594.
Gr5ger, Max.
(191 1) Z.anorg.Chem., 70, 135.
Groschuff, £.
(1901) Ber., 34, 3318.
(1903) Ber., 36, 1791, 4351.
(1908) Z.anorg.Chem., 58, 102, 113.
(1910) Chem.Weekblad., 7, 687.
(191 1) 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. >
(191 2) Thesis, Lausanne.
Guerin, G.
.(1913) J.pharm.chim., [7), 7, 438.
(191 3) rnarm.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, loi.
Gurwitsch, L.
(1914) Z.physik.Chem., 87, 329.
Guthrie.
(1875) Phil.Mag.,
(1876) Phil.Mag.,
(1878) Phil.Mag.,
(1884) Phil.Mag.,
4I, 49, 210.
5], ii 366.
5l» 6, 40.
5l» 18, 30, 504.
Guthrie. A.
(1901} J.SocChem.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., I2], 33, 433.
Bamberger, Anna.
(1906) Z.anorg.Chem., 50, 427.
Hamburger. E.
(191 1) Arch.ge8.Physiol.(Pfluger's),
143, 187.
von Hammel, A.
(1915) Z.physik.Chem., 90, 121.
Hampdiire, C. H. and Pratt. W. R.
(191 3) 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.
(191 1 ) Ber., 44, 2006.
Hantzsdi, A. and Sebalt, F.
(1899) Z.physik.Chem., 30, 258-99.
mtzsdi, A. and Vagt, A.
(1901) Z.physik.Chem., 38, 705-742.
; ^.pnys
;,w:d.
(19H) 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.
(191 1 ) T.Am.Chem.Soc., 33, 1827-36.
Harrass, Paul.
(1903) Arch.intemat.Pharmacodyamie
et Therapie, 11, 431-463.
Hartley. H.
(1908) J.Chem.Soc.(Lond.), 03f 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.
(1913) 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
Hftrttey. H. and Thomas.
(1906) J.Chein.Soc.(Lond.)i 89, 1028.
Haalam.
(1886) Chem.News., 53, 87.
Haaselblatt, M.
(19 1 3) Z.physiicChem., 83, 1-39.
Hatcher, R. A.
(1902) Am.Jour.Pharm., 74, 136.
Hatcher, W. H. and Skirrow, F. W.
(191 7)J.Am.Chem.Soc., 39,1939-1977.
V. Hauer.
(1858) T.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.
(1909a) Z.angew.Chem., 22, 484.
(191 2) Z.anorg.Chem., 78, 75-94.
Heath, W. P.
(191 5) Privately Printed, Atlanta,
Ga.
Hehner. O. and Mitchell, C. A.
(1897) J.Am.Chem.Soc., 19, 40.
van der Ueide.
(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.
(191 1) 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.
(191 2) Landolt & Bornstein's,
" Tabellen," 4th Ed., 602.
Henry.
(1884) Compt.rend., 99, 1157.
Herold, J.
(1905) Z.Elektrochem, ii, 417.
Herrmann, Gottfried.
(191 1) 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.
(1910a) Z.anorg.Chem., 66, 93, 358.
(1910b) Z.anorg.Chem., 65, 341-4.
Herz, W.
(1910c) Z.anorg.Chem., 67, 365.
(191 1 ) Z.anorg.Chem., 70, 70, 170.
(1911a) Z.anorg.Chem., 71, 206.
(1911b) Z.anorg.Chem., 72, 106.
(1911-12) Z.anorg.Chem., 73, 274.
(191 7) 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.
(191 1 ) Z.anorp;.Chem., 71, 255.
Herz, W. and Fischer, H.
(1904) Ber., 37, 4747.
(1905) Ber., 38, 1 140.
Herz, W. and Knoch.
(1904) Z.anorg.Chem., 41, 319.
(1905) Z.anore.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., xi, 818.
Herz, W. and Muhs, G.
(1903) Ber., 36, 3717.
Herz, W. and Paul, w.
(191 3) Z.anorg.Chem., 82, 431.
(19 1 4) 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.
▼on Hevesy, Geo.
(1900) Z.phy8ik.Chem., 73, 537.
(1909) Z.Elektrochem., 15, 529.
(191 1) Phys.Ztschr., 12, 1214.
(1912) J.Phys.Chem., 16, 429.
von Hevesy, G. and R6na, E.
(191 5) Z^hysik.Chem., 89, 303.
Hicks, W. B.
(19 '5) J.Am.Chem.Soc., 37, 844.
Hildebrand, J. H., EUefson, E. T. and
Beebe, C. W.
(191 7) 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.
(191 6) Z.angew.Chem., 29, I, 57-9.
(1916) Chem.Abs., xo, 1924.
798
AUTHOR INDEX
ffinrichsen. F. W. and Sachsel, £.
(1904-05) Z.physik.Chem., 50, 81-99.
His, W. Jr. and Paid, T.
(1900) Z.physiol.Chem.y 31, 1-42,
64-78.
Hissink. D. J.
(1900) Z.physik.Chem., 33, 557.
Hitchcock, F. R. M.
(1895) J.Am. Chem.Soc., 17, 529.
▼an't Hoff, J. H.
(1901) Sitzber.k.Akad.Wiss. (Berlin),
p. 1035.
(1905) Z.anorg.Chem., 47, 247.
(1912) '* Untersuchungen Qber die
Bildungsverhaltnisse der
Ozeanischen Salzablager-
ungen, inbesondere des
Staasfurter Salzlagers."
von J. H. van't Hoffet al
Herausgegeben von H.
Precht & E. Cohn.
(Leipzig, 1912).
▼an't Hoff, J. H. and Goldschmidt, H.
(1895) Z.physik.Chem., 17, 508.
van*t Hoff, J. H. and Meyerhoffer, W.
(1898) Z.physik.Chem'., 27, 75.
(1899) Z.physik.Chem., 30, 64-88.
van't Hoff, J. H. and Kenrick,.F. B.
(1912) " (3zeanischen Salzablagerun-
gen," pp. 57-40.
Hoffmann, Fr. and Lauogbeck, K.
(1905) Z.physik.Chem., 51, 303, 393,
412.
Hofmann, K. A., H5bold, K. and Quoos.
(1911-12) Liebig's Ann., 386,304-
317.
Hofmann, K, A. and H5bold, K.
(1911) Ber., 44, 1776.
Hofmann, K. A., Kirmireuther, K. and
Thai, A.
(1910) Ber., 43, 188.
Hofman, JL A., Roth, R., H5bold, EL
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.
(1898a) Z.physik.Chem., 27, 315.
Holde, D.
(1910) Z.Elektrochem., x6, 442.
Holland, A
(1897) Ann.chim.anal., 2, 243.
HoUeman, 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.
(191 3) Rec.trav.chim., 32, 136.
(1914) Rec.trav.chim., 33, 6-29.
HoUeman, A F. and van den Arend, J. £.
(1909) Kec.trav.chim., 28, 411.
Holleman, A. F. and Antttsch, A C.
(1894) Rec.trav.chim., 13, 293.
Hollenian, A. F. and de Bruyn, B. R.
(1900) Rec.trav.chim., 19, 83, 191,
365.
Holleman, A. F. and Caland, P.
(191 1 ) Ber., 44, 2506.
Holleman, A. F., Hartogs, J. C, and
van der Linden, T.
(191 1) 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.
(191 1) Rec.trav.chim., 30, 318.
Holleman, A. F. and PoUak, J. J.
(19 10) Rec.trav.chim., 29, ^9,
Holleman, A F. and Rinkes, I. J.
(191 1) Kec.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-
iio.
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.
Homfrav, L 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.CoU.Sci. (Kyoto), i,
49-55.
Horn, D. W.
(1907) Am.Chem.Jour., 37, 471.
Horn, D. W. and Van Wagener.
(1903) Am.Chem.Jour., 30, 347.
Houston and Trichbome.
(1890) Brit. Med. Jour., 1063.
Howe, Jas. L.
(1894) J.Am.Chem.Soc., i6, 388.
Hudson, C. S. «
(1904) J.Am.Chem.Soc., 26, 1072.
(1908) J.Am.Chem.Soc., 30, 1767-83.
Hudson^ C. S. and Yanovtty, £.
(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
Hfilner, G. tiid Kolz.
(1895) J.prakt.Chem., 38, 256.
Hnlett, G. A.
(1901) Z.physik.Chein., 37, 406.
Huletty G. A. and Allen, L. K.
(1902) J.Am.Chem.Soc., 24, 674.
Hunt
(1870) Am.Jour.Sci., [2], 40, 154.
Hattig, Giistav, F.
(19 1 4) Z.physik.Chem., 87, 144.
niinsworth, B. and Howard, A.
(1884) Phil.Mag., [5], 18, 124.
Imadsti, A.
(1911-12) Mem.Coll.Sci.Eng. (Ky-
oto) p 3, 257-63.
IngUs, J. K. H.
{'903) J.Chem.Soc.(Lond.), 83, loio.
Lnnng and Toung.
(1888) J.Chein.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.
▼an Itallie, E. J.
(1908) Z.anorg.Chem., 60, 358-65.
▼an Iterson-Rotgans, J. W.
(191 3) Chem.Weekblad., 10, 920-37.
(1914) Z.physik.Chem., 87, 305.
Iwaki, J.
(1914) Mem.Coil.Sci.(Kyoto), 1,81-8.
Iwig and Hecht
(1886) Liebig's Ann., 233, 167.
Jackson, R. F.
(1914) J.Am.Chem.Soc., 36. 2350.
(1914) Bull.BureauStandards, 2, 331-
345-
Jacobs, W.
(191 7) 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.), 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 Doombosch, H. J. D.
(191 2) Z.anorg.Chem., 75, 261.
Jaeger, F. M. and van Klooster, H. S.
(1912) Z.anorg.Chem., 78, 245.
Jaeger, F. M. and van Eregten, J. R. N.
(1912) Proc.k.Akad.Wet.(Amst.), 14,
733.
Jaeger, F. M. and Menke, J. B.
(1912) Z.anorg.Chem., ^ 241-260.
(1912) Proc.k.Akad.Wet.(Amst.), 14,
Jaenecke, £.
(1908) Z.physik.Chem., 64, 343.
(191 2) Z.physik.Chem., 80, i.
Jakowkin, A. A.
(1895) Z.physik.Chem., 18, 588.
(1896) Z.physik.Chem., 20, 38.
(1899) Z.phy5ik.Chem., 29, 630.
James, C. and Holden, H. C.
(1913) J.Am.Chem.Soc., 35, 559.
James, C. and Pratt, L. A.
(1910) J.Am.Chem.Soc., 32, 873.
James, C. and Robinson, J. £.
(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.
(191 6) J.Am.Chem.Soc., 38, 1499.
Jantsch. &.
(1912} Z.anorg.Chem., 76, 321.
Jantsch, G. and Grflnkraut, A.
(19 1 2-1 3) 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.
(191 1 ) Z.anorg.Chem., 70, 86-134.
Jensen, H. R.
(191 3) Pharm.Jour.(Lond.), 90, 658-
60.
Jo, Inohiko.
(191 1) Mem.coll.sci.Eng. (Kyoto), 3,
41-9, 212.
(191 2) Tokyo Chem.Soc,, 33, No. 7,
July.
Joannis. A.
(1882) Ann.chim.phys., [5], 26, 489.
(1906) Ann.chim.phys., [8J, 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., 35, 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.
(191 5) J.Am.Chem.Soc., 37. 241.
(19 1 6) Trans. Am. Elect rochem.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.,
i4» 27-9.
Jones, W. J.
(191 1 ) J.Chem.Soc.(Lond.)> 99» 392.
de Jong, A. W. K.
(1909) Rec.trav.chim., 28, 343.
(1912) Rec.trav.chim., 31, 256.
JOrgensen.
{1879) J.prakt.Chem., [2], 20, 195.
(1884) J.prakt.Chem., 12], 30, i.
(1890) J.prakt.Chem., [2], 42, 208.
Joulin.
(1873) Ann.chim.phys., [4], 30, 260.
Joumiaux, M.
(19 12) BuU.soc.chim. (Paris), [4], 11,
129, 516, 546-52.
Joyner, R. A.
(191 2) Z.anorg.Chem., 77, 108.
Jun^eisch, E.
(1912) Compt.rend., 155, 801.
Jungfleisch, E. and Lan<meu, Ph.
(1914) Ann.chim., 2, 1-56, 333.
(1914a) 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) BuU.soc.chim., 13, 460.
E^ahlenberg, Ia and Brewer, R. K.
(1908) J.Phys.Chem., 12, 283-9.
E^ahlenberg, L. and Erauskopf, F. C.
(1908) J.Am.Chem.Soc., 30, 1 104-15.
E^ahlenberg, L. and Wittich, W. J.
(1909) J.Phys.Chem., 13, 421-5.
E^ahlukow, I. and Sachanow, A.
(1909) J.Russ.Phys.Chem.Soc., 41,
1755-
KarandeefF, B.
(1909) Zentralbl.Min.Geol., p. 728.
(191 o) Z.anorg.Chem., 68, 188.
Karl, G.
(1910) Z.anorg.Chem., 68, 57.
Earplus.
(1907) Dissertation, Berlin.
Landolt & Bernstein'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.
(191 1) Proc.Roy.Soc.(Lond.), A, 85,
200-19.
Kendall. J.
(1912) Pjiil.Mag. [6], 3}, 9^8.
(1914) J.Am.Chem.Soc., 36, 1722.
(1914a) J.Am.Chem.Soc., 36, 1222.
(1916) J.Am.Chem.Soc., 38, 1309.
Kendall. J. and Booge, J. £.
(1916) J.Am.Chem.Soc., 38, 1712.
Kendall, J. and Carpenter, C. D.
(1914) J.Am.Chem.Soc., 36, 2502.
Kendall. J. and Gibbons, W. A.
(191 J) J.Am.Chem.Soc., 37, 149.
KeppisL
• (1888) Monatsh.Chem., 9, 589.
Kemot, G., d'Agostino, E. and Pelle-
grino, M.
(1908) Gazz.chim.ital., 38, I, 532-54.
Kemot, G. and Pomilio, M.
(1912) Rend.accad.sci.fis.nat.(Nap-
oli), [3I, 17, 353-8.
Ketner.
(1901-02) Z.physik.Chem., 39, 645.
Keves, D. B. and Hildebrand, J. Bl.
(1917) J.Am.Chem.Soc., 39, 2129.
Keves, D. B. and James, C.
(1914) J.Am.Chem.Soc., 36, 634.
King, Chas. A. and Narracott, P.
(1909) Analyst, 34, 436-8.
E^ing, H. and Orton, K. P. J.
(191 1) J.Chem.Soc.(Lond.), 99, 1381.
King, Harold and Pyman, F. L.
(1914) J.Chem.Soc.(Lond.), 105,
1238-59.
Kirschner, A.
(19 1 2) z.physik.Chem., 79, 247.
Klaus.
(1905) Phys.Ztschr., 6, 820.
Klein, O.
(19 1 2) Z.anorg.Chem., 74, 158.
Kleven.
(1872) Chem.Centralbl., 434.
Klobbie, E. A.
(1897) Z.physik.Chem., 24, 623.
▼an Klooster, H. S.
(1910-11) Z.anorg.Chem., 69, 122,
135-57.
(1912-1 3) Z.anorg.Chem., 79, 223-9.
(191 7) J.Phys.Chem., 21, 513-18.
Klose, G.
(1907) Archiv.Internat.Pharmacody-
namie et Therapie, 17,
459-63-
Knietsch, R.
(1901) Ber., 34, 4099.
EInopp.
(1904) Z.physik-Chem., 48, 97-108.
EInoz, 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.phy8ik.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.
KOhier.
(1879) Z.anal.Chem.p 18, 242.
KOhler.
(1897) Z.Ver.Zuckerind., 47, 447.
Kohlraosch, 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-^-
(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 Timmennans, J.
(i9i3)Proc.k.Akad.Wet.(Amst.), 1021.
Kolb.
(1872) BuU.soc.ind.Mulhouse, 222.
de Kolossovsky, N.
(191 1) Bull. soc.chim. (Paris), [4], 9,
632-7.
(191 1) Bull.soc.chim.(Belg.), 25, 183,
235-
Kolfhoff, L M.
(191 7) Chem.Weekblad., 14, 1081.
Konig.
(1894) Monatsh.Chem., 15, 23.
de Koninck, L. L.
(1907) B uii. soc.chim. (Belg.), 21, 141.
Konowalow, D.
( 1 898) Jour. Russ. Phys.Chem.Soc. ,
[4I, 30, 367.
(1898) Chem.Zentralbl., II, 659.
(1899a) Jour. Russ. Phys.Chem.Soc.,
3i» 910.
(1899b) Jour. Russ. Phys.Chem.Soc.,
3ii 985-
(1900) Chem.Zentralbl., I, 646.
(1900b) Chem.Zentralbl., I, 938.
(1903) Ann.Phys.(Wied.), [4], 10,375,
Koopal, S. A.
(191 1) Dissertation, Leyden, p. 128.
(191 1) "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 Blnmenfhal, R.
(1907) Z.anorg.Chem., 53, 228-67.
Sloppel, J. and Cahn, M.
(1908) Z.anorg.Chem., 60, 53-112.
Koppel-Gumpezy.
(1905) Z.physik.Chem., 52, 413.
S^ppel, J. and Holtkamp, H.
(19 lo) Z.anorg.Chem., 67, 274.
Koppel-Wetzel.
(1905) Z.physik.Chem., 52, 395.
Korreng, E.
(19 1 4) Neues Jahrb.Min.Geol.(Beil
Bd.), 37, 51-124.
(191 5) Z.anorg.Chem., 91, 194.
Krasnicld.
(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,
1 125.
(1908) Jahrber.k.geol.Reichsanstalt
(Wien), 58, 662.
(1909) "The Use of Thermic Analysis
fort he 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.
(1910a) Monatsh.Chem., 31, 275.
(191 1 ) Monatsh.Chem., 32, 609.
( ) . Sitzber.k.Akad.Wiss.(Wien),
120, lib, 329.
Kremann, R. et ai.
(1908) Monatsh.Chem., 29, 863-91.
Kremann, R. and Borjanovics, V.
(1916) Monatsh.Chem., 37, 59-84.
Kremann, R., Daimer and Beunesch.
(191 1) 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 Htittinger, K.
(1908) Jahrber.k.Geol.Reichsanstalt
(Wien), 58, 637.
Kremann, R. and Janetzky, £.
(1912) Monatsh.Chem., 33, 1055-62.
Kremann, R. and Kerschbatmi, 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.Chera., 33, 1205.
902
AUTHOR INDEX
Kremann, R. and Rodemund, Hi
(19 14) 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. IT^scho, 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.
(1856a) Pogg.Ann., 97, 5.
(1858) Pogg.Ann., 103, 57, I33, 165.
(1858) Pogg.Ann., 104, 133.
(i860) PoggJVnn., Ill, 60.
Kreusler and Herzfaold.
(1884) Ben, 17, 34.
Krug, W. H. and Cameron, F. K.
(1900) J.Phys.Chem., 4, 188.
Krug, W. H. and McBlroy, 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.
(191 2) Z.physik.Chem., 79, 667.
Krvm, V.
(1909) J.Russ.Phys.Chem.Soc., 41,
382-5; Chem.Zentr., II, 681.
Kulisch.
(1893) Monatsh.Chem., 14, 567.
KultasdiefF.
(1903) Z.anorg.Chem., 35, 187.
Ktmipf.
(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) Zj)hysik.Chem., 24, 441-467.
(1897a) Z.physik.Chem., 23, 93, 547,
67J.
(1898) Z.physik.Chem., 25, 419-440.
Kumakov, If. S. and Efrenov, N. N.
(191 2) Jour.Russ.Phys.Chem.Soc.,
44, 1992-2000.
(1912) Ann.Inst.Polyt.(Petrograd),
18, 105.
Kumakov, J.,Krotkoy, D. and Oksman,
M.
(1915) Jour.Russ.Phys.Chem.Soc.,
47, 558-88.
Kumakov, H. and Kviot, L
(1913) Ann. Inst. Polyt.(Petrograd),
20, 664.
Kumakov, N. S. and Solovev, V.
(1916) J.Russ.Phys.Chem.Soc., 48,
1338.
Kumakov, N. S. and Wrzesnewsky.
J.B.
(1912) Z.anorg.Chem., 74, 89.
Kurnakov, N. S. and Zemcznzny.
(1907) Z.anorg.Chem., 52, 186.
Kaster, 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.
Kfister, F. W. and Heberlein, E.
(1905) Z.anorg.Chem., 43, 56.
Kiister, F. W. and Kremann, R.
(1904) Z.anorg.Chem., 41, 19.
Kaster and Thiel.
(1899) Z.anorg.Chem., 2X, 116.
(1903) Z.anorg.Chem., 33, 139.
Kaster, F. W. and WOrf el, 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], j5, 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 Sobedd.
(1910) Ber., 43, 2375.
Lai De, R.
(191 7) J.Chem.Soc.(Lond.), iii, 55.
Lami, Pio.
(1908) Chem.Zentr., II, 755.
(1908) Boll.chim.farm., 47, 435-441.
Lamouroux, F.
(1899) Compt.rend., 128, 998.
Lazny.
(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 Bdmstein.
(1912) Physikalisch-Chemische Tab-
cllen, 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.), 3I1388.
803
AUTHOR INDEX
Lautz, H.
(191 3) Z.physik.Chem., 84. 633.
Laws, B. G. and Sidgwick, N. V.
(191 1) J.Chem.Soc.(Lond.),99, 2088.
Leader, J. W. and Mukerji, J. M.
(1913) Mem. Dept.Agr. (India), Chem.
Ser., 3, 177-204.
Leather, J. W. and Sen, J. N.
(1909) Mem.Dept.Agr.(India),Chem.
Ser., 1, 117-131.
(1914) Mem. Dept.Agr. (India), Chem.
Ser., 3, 205-34.
Lebeau, P.
' (1906) Ann.chim.phys., [8], 9, 482-4.
(191 1 ) Compt.rend., 152, 440.
Lebedew, P.
(191 1 ) Z.anorg.Chem., 70, 302, 316.
LeBUnc, M. and Novotny, K.
(1906) Z.anorg.Chem., 51, 181-201.
LeBianc, M. and Noyes, A. A.
(1890) Zjshysik.Chem., 6, 386.
LeBianc, M. and Schmandt, W.
(191 1) 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.
(191 1) Z.physik.Chem., 77, 311.
▼an 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., 11 1, 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) BuU.soc.chim., [3], ix, 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.
(191 7) 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.
Lidi^, D. M.
(1903) J.Am.Chem.Soc., as, 474.
Udoff.
(1893) BuU.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) BuIl.soc.chim.Belg., 23, 179-
200.
lincoln, A. T.
(1900) J.Phys.Chem., 4, 176.
(1904) J.Phys.Chem., 8, 251.
van der liinden, T.
(191 2) Ber., 45, 237.
(1916) Arch.Suikennd, 24, 11 13— 28.
(191 7) Chem.Abs., 11, 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., 11, 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, B.
(1909) Compt.rend., 149, 284-6.
(1911) J.pharm.chim., [7], 3, 377-385-
(1911) J.pharm.chim., [7], 4, 193-7.
(191 1) Ann.fals., 4, 302-5.
L5wel.
(1851) Ann.chim.phys., [3], 33, 382.
804
AUTHOR INDEX
LOwenherz, R.
J1894) Z.physik.Chem., 13, 479.
1895) Z.physik.Chem., 18, 82.
I1898) Z.physik.Chein., 25, 395-410.
Lubarsdi.
(1889) Wied.Ann.Physik., [2], 37, 525.
Lubavin.
(1892) J.Russ.Ph^ Chem.Soc.p 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, 12 13.
Lomsden, J. S.
(1902) J.Chem.Soc.(Lond.), 81, 355.
(1905) J.Cheni.Soc.(Lond.), 89, 90.
Lund6n, Harold.
(1905-6) Z.physik.Chem., 54, 564.
(19 1 3) Medd.K.Vetenskap8akad.
Nobelinst., 2, No. 15.
(191 3) Chem.Abs., 7, 2887.
Luther, R. and Leubner, A.
(1912) Jj)rakt.Chem., [2]. 85, 314.
(1912a) Z.anorg.Chem., ^4* 3^9.
Lutz, O.
(1902) Ber., 35, 2462.
(1910) Ben, 43, 2637.
van Maarseveen, G. (Goldschmidt, H.)
(1898) Z.physik.Chem., 25, 90-99.
Maass, O. and Mcintosh, D.
^1912) J.Am.Chem.Soc., 34, 1279.
(1913) J.Am.Chem.Soc., 35, 538.
Maben.
(1883-84) Pharm.JoUr.(Lond.), [3],
I4i 505.
MacAdam, D. J., Jr. and Pierle, C. A.
(1912) J.Am.Chem.Soc., 34, 604.
MacArthur, C. G.
(191 6) 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.
(191 1 ) J.Am.Chem.Soc., 33, 468-473.
McCoy, H. N. and Test, Chas. D.
(191 1 ) J.Am.Chem.Soc., 33, 473-6.
McCrae, J. and li^son, W. B.
(1903) Z.anorg.Chem., 35, 11.
M'David, J. W.
(1909-10) Proc.Roy.Soc. (Edin-
burgh), 30, 440-7.
McDaniel, A S.
(191 1 ) J. Phys.Chem., 15, 587^10.
McDennott, F. Alex.
(191 1) J.Am.Chem.Soc., 33, 1963.
McDonnell, C. C. and Smith, C. M.
(1916) J.Am.Chem.Soc., 38, 2366.
Mcintosh, 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 Mailf ert.
(1894) Compt.rend., 1x9, 951.
Maigret.
(1905) Bull.80c.chim. [3], 33, 631.
Mallet.
(1897) Am.Chem.Jour., 19, 807.
Malvano, L.
(1906) Z.anorg.'Chem., 48, 446.
Malvano, L. andf Mannino.
(1908) Atti accad.Lincei, [5], 17, II,
484.
Mameli. £. and Mannessier, A.
(191 3) 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.
(191 6) 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., 37i 1041.
Marden, J. W.
(1914) J.Ind.Eng.Chem., 6, 315-20.
(1916) J.Am.Chem.Soc., 38, 310.
Marden, T. W. and Dover, Mary V.
(1916) J.Am.Chem.Soc., 38, 1239.
(191 7) J.Am.Chem.Soc., 39, 4.
Marie, C. and Marquis, R.
(1903) Compt.rend., 136, 684.
Marignac.
J1853) Ann.chim.phys., [3], 39, 184.
ji86i) 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 Strutitiers. 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,i074-
1085.
805
AUTHOR INDEX
Manhattt H. and C«meroii, A. T.
(1907) J.Chem.Soc.(Lond.), gi, 1522.
Mascarelli. L.
(1906) Atti accad.Lincei, [5], 15, I,
192; 11.459-
(1906a) Atti accad.(Lincei), [5], 15,
192.
* (1906a) Gazz.chim.ital., 36, II, 880-
893.
(1908) Atti accad.Lincei, [5], 17, I,
29.
(1909) Gazz.chim.ital., 30. I, 251-84.
BCascarelli, L. and AscoU, tJ.
(1907) Gazzxhim.ital., 37^ I, 125.
Mascarelli, L. and Constantino, A.
(1909) Atti accad.Lincei, [5], xS, II,
104.
(1910) Gazz.chim.ital., 40, Ii 4i-
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.
(19 1 5) Atti accad.Lincei, [5], 24, II,
94.
Massink, A.
(1916) Z.physik.Chem., 12, 351-80.
(191 7) Chem.Weekblad., 14, 756.
Massol and Maldes.
(1901) Compt.rend., 133, 287.
Masson, I.
(1912-13) Proc.Roy.Soc.(Edin.), 33,
64-8.
Masson, T. J. Onne.
(191 1) J.Chem.Soc.(Lond.). 99» 1132.
(1912) J.Chem.Soc.(Lond.) loi, 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.
(191 7) J.Phys.Chem., 21, 269-74.
Mathews, J. H. and Spero, S.
(191 7) 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-
(1909a) 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.Fcnd., 58, 81.
Mayer.
(1856) Liebig's Ann., 98, 193.
Mayer, O.
(1903) Ber., 36, 1741.
Mazatto.
(1891) Nuovo.cimento, [3], 29, 21.
Meerbiurg, 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.
(191 1) Chem.Zentralbl., I, 1036.
Meentm-Terwogt.
(1905) Z.anorg.Chem., 47, 203.
Mees, C. E. K. and Piper, C. W.
(191 2) Photogr.
Photogr.
Photogr..
our., 33, 227.
our., 36, 2^4.
our., 52, 2'>i-37.
(1891) Liebig's Ann., 261, 360.
Melcher, A. C.
(1910) J.Am.Chem.Soc., 32, 50-66.
Meldrum, R.
(191 3) Chem. News., 108, 199.
MeUor, J. W.
(1901) J.Chem.Soc.(Lond.), 79, 225.
Meneghini, D.
(19 1 2) Gazz.chim.ital., 42, II, 474.
Menge, Otto.
(191 1) Z.anorg.Chem., 72, 169-218.
Menke, J. B.
(19 1 2) Z.anorg.Chem., 77, 283.
Menschutkin, B. N. (see pp. 379 and
391).
(1905) Mem.St. Petersburg Polyt.Inst.,
4, 75-101.
(i906)Mem.St.Petersburg Polyt.Inst.,
5i 355-388.
(1907) Z.anorg.Chem. 52, 9, 155; 53,
26.
(1907a) Z.anorg.Chem., 54, 89-96.
( 1908) Mem.St . Petersburg Polyt. I nst .,
9, 200-222.
(i909)Mem.St.Petersburg Polyt.Inst.,
II, 261, 567; 12, I.
(1909) Z.anorg.Chem., 61, 106, 113.
{ 1 9 10) Mem.St .Petersburg Polyt. Inst.,
13,1,263,411,565; 14,251.
( 1 9 1 1 ) Mem .St . Petersburg Pol}^ .1 nst .,
15, 65, 397, 613, 647, 757.
(i9i2)Mem.St.Petersburg Polyt.Inst.,
16, 33, 397.
Menzies, A. W. C. and Dutt, N. N.
(191 1) J.Am.Chem.Soc., 33, 1266.
Menzies, A. W. C. and Humphrey, E.C.
(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.
Mescherzersld.
(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.
(191 1) Ben, 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) Ben, 8, 998.
Meyerhoffer, W.
(1904) Landolt and Bornstein '* Tab-
ellen," 4th Ed., 1912, p. 486.
(1905) Z.physik.Chem., 53, 513-603.
(191 2) Landolt and Bornstein "Tab-
ellen," 4th Ed., p. 481.
Meyerhoffer, W. und Saunders.
(1899) Z.physik.Chem., 28, 466; 31,
382.
Michael, Arthur.
(1901) Ben, 34, 3641, 3656.
Michael, Arthur and Gamer, 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.
(1908a) J.Chem.Soc.(Lond.), 93, 931.
Bfilbauer, J.
(1912-13) J.prakt.Chem., [2], 87, 398.
Milikau. J.
(1916) Z.physik.Chem., 92, 59-80.
Miller, W. Lash and McFherson, R. H.
(1908) J.Phys.Chem., I3, 709.
Mills, w. H., Parker, H. V. and
Prowse, R. W.
(1914) }.Chem.Soc.(Lond.),i05,i54i.
Mills, R. V. and WeUs, R. C.
(191 8) Bull.U.S.Geol.Sur/ey, No.
693, p. 72.
Miolati, A
(1892) Z.physik.Chem., 9, 651.
Mitsdierlich.
(1832) Pogg.Ann., 25, 301.
Moissan, H.
(1882) Buil.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, loio.
(1904) Ben, 37, 2088.
Moles, B. and Jimeno, £•
(191 3) Anales.soc.espan.fis.quim., ii,
393.
Moles, B. and Marquina, M.
(19 14) Anales.soc.espan.fis.quim., 12,
,^ , 383-93.
MOnkemeyer.
(1906) N.Jahrb.Min,Geol.(Beil.Bd.),
22, I.
Moody, G. T. and Leyson, L. F.
(1908) J.Chem.Soc.CLond.), 93, 1767.
Moore, B. and Roaf, H. B.
(1904) Proc.Roy.Soc.(Lond.), 73,
382-412.
Moore, B., "^nison, F. P. and Hutchin-
son, L.
(1909) Biochem.Jour., 4, 347.
Moore, T. S. and Winmill, T. F.
(1912) }.Chem.Soc.(Lond.), 101,1662.
Morey, Geo. W.
(1917) J.Am.Chem.Soc., 39, 1173-
1229.
Morgan. T. L. R. and Benson, H. K.
(1907) J.Am.Chem.Soc., 29, 11 76.
(1907) Z.anorg.Chem., 55, 356.
Morgan, T. C. and James, C.
(1914) J.Am.Chem.Soc., 36, 10-16.
Morell, R. S. and Hanson, B. 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.
Mouf gang, B.
(191 1) Wochschr.Brau., 28, 434-6.
(191 1) J.Soc.Chem.Ind., 30, 1210.
Muchin. G.
(1913) " Solubility of Calcium Iodide
m Organic Solvents,'* Pamphlet,
45 PP* ^nd 12 charts, KharkofT,
191 3. (Reprint in the Russian
language received from author.)
See also Trav.sco.sci. physic.
Chem. Univ. KharkofT 39 fasc.,
24, 1-49, 1913.
Mulr.
(1876) J,Chem.Soc.(Load.)>a9} 857.
807
AUTHOR INDEX
Mulder, G. J.
(1864) Scheikundige Verhandelingen
en Onderzoekingen, Vol. 3, Pt. 2,
fiijdragen tot de Geschiedenis
van Het Scherkungig Gebonden
Water, Rotterdam, 1864.
Mulder, Gay-Lussac, Etard.
(1894) Ann.chim.phys., [7], a, 528.
Mueller, J. H.
(1917) J.Biol.Chem., 30, 39-40.
Mueller, P. and Abegg, R.
(1906) Z.physik.Chem., 57, 514.
MiiUer, C.
(1910) N.Jahrb.Min.Geol.(Beil.Bd.),
30, I.
(1912-13) Z.physik.Chem., 81, 483-
503.
Milller.
(1887) Compt.rend., 104, 992.
(1889) Wied.Ann.Physik., [2], 37, 29,
(1892) Ann.chim.phys., [6], 37, 409.
MiiUer, H.
(1912) J. Chem.Soc.(Lond.), 101,2400.
MiiUer, W.
(1903) Apoth.Ztg., 18, 208, 249, 257.
Muraro. F.
(1908) Gazz.chim.ital., 38, 1, 427; II,
507.
Muthmann and Kuntze.
(1894) Z.Kryst.Min., 23, 368.
Muthmann and RdUg.
(1898) Z.anorg.Chem., 16, 455.
(1898) Ber., 31, 1728.
MyUus, F.
(1901) Ber.. 34, 2208.
(191 1) Ber. 44, 1315-
(191 1) Z.anorg.Chem., 70, 209.
MyUus, F. and Dietz.
(1901) Ber., 34, 2774.
(1905) Z.anorg.Chem., 44, 217.
(1905) Ber., 38, 921.
MyUus, F. and F5rster.
(1889) Ber., 22, 1 100.
(1892) Ber., 25, 70.
MyUus, F. and Funk, R.
(1897) Ber., 30, 1718.
(1900) Wiss.Abh.p.t.Reichsanstalt, 3,
451.
(1900J Ber., 33, 3686.
MyUus, F. and von Wrochem, J.
(1900) Wiss.Abh.p.t.Reichsanstalt, 3,
462.
(1900) Ber., 33, 3689.
Nacken, R.
(1907a) Nachr.kgl.Ges.Wissenschaft
(Gottingen), 602.
(i907b)Jahrb.Min.Geol.(Beil.Bd.),24,
I.
(1907c) Zentralbl.Min.Geol., 262, 301.
(1910) Sitzber.kgl.preuss.Akad.Wis.,
1016-26.
Nagomow, N. N.
(191 1 ) Z.physik.Chem., 75, 578.
Nanty, T.
(191 1 ) 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.
(191 1 ) 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.
(19 1 2) Analyst., 37, 399.
Nemst, 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 Niementowsld, S. and von Rosz-
kowski, T.
(1897) Z.physik.Chem., 22, 146.
Noelting, F.
(19 10) Ann.chim.phys., [8], 19, 486.
Nordenskjold and Lindstrom.
(1869) Pogg.Ann., 136, 314.
Noss, F.
(191 2) 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.
Noves, A. A. and Abbott, C. G.
(1895) Z.physik.Chem., 16, 130.
Noves, A. A. and Boggs, C. R.
{191 1 ) J.Am.Chem.Soc., 33, 1650.
Noyes, A A and Chapin, £. S.
(1898) Z.physik.Chem., 27, 443.
(1899) J.Am.Chem.Soc., 2Z, 513.
Noyes, A. A. and Clement
(1894) Z.physik.Chem., 13, 413.
Noves, A. A. and Farrel, F. S.
(191 1) J.Am.Chem.Soc., 33, 1654.
Noves, A. A. and HaU, F. W.
(1917) J.Am.Chem.Soc., 39, 2529.
Noves, 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
Koyei , A. A. aad Schwartz, D.
(1 898) Z.physik.Chem., 27, 279-284.
(1898) J.Am.Chem.Soc., 20, 744.
Noyes, A. A. and Seidenslicker.
(1898) Z.physik.Chein., 27, 359.
Noyes, A. A. and Stewart, M. A.
(191 1) J.Am.Chem.Soc., 33, 1658.
Noves, A. A. and Whitcomb, W. H.
{1905) J.Am.Chem.Soc., 27, 756.
Odaira, I.
(1915) Mem.Coll.Sci.(Kyoto), 1,324,
330.
Oddo, B.
(1913) Gazz.chim.ital., 43, II, 275.
Okada, K.
(i9i4)Mem.Coll.Sci.(Kyoto), 1,95-
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], 27, II,
512, 584, 717.
(1909) Atti accad.Lincei, [5], x8, II,
96.
(191 1 ) Atti accad.Lincei, [5], 20, I,
470-4.
(1912) Atti accad.Lincei, [5], 2Z, 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.
(191 1 ) J.Chem.Soc.{Lond.),99, 1192.
Osaka, Y.
(1903-8) Mem.Coll.Sci.Eng. (Kyoto),
ii 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 1 ) Mem.Coll.Sci.Eng. (Kyoto),
3i58.
(191 1) J.Tok.Chem.Soc., 32, 870.
Osaka, T. and Abe, R.
(191 1) Mem.Coll.Sci.Eng. (Kyoto), 3,
5^-4.
>k.(
(191 1 ) J.Tok.Chem.Soc., 32, 446.
Osborne, T. and Harris, L 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.
(1907) J.pharm.chim., [6], 26, 162.
Ost
(1878) J.prakt.Chem., [2), 17, 232.
Oswald, M.
(1914) Ann.chim., 1, 57-79.
(1912) Compt.rend., 155, 1504.
(1912) 8th Int.Cong.Appl.Chem., 2,
205.
Oudemans, A. C. Jr.
(1872) Z.anal.Chem., ix, 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], Z2, II,
160.
de Paepe, Desir6.
(191 1) BuU.aoc.chim.Belg., 25, 174.
Paietta, 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.
(1893a) J.Russ.Phys.Chem.Soc., 25,
262.
(1894) Z.anorg.Chem., 5, 490.
Parker, B. G.
(19 1 4) J.Phys.Chem., 18, 653.
Parmentier.
(1887) Compt.rend., Z04, 686.
(1892) Compt.rend., 114, 1002.
Parravano^ N.
(1909) Uazz.chim.ital., 39, II, 58.
Parravano, N. and Calcagni, G.
(1908) Atti accad.Lincei, [5], 17, I,
731-8.
(19 10) Z.anorg.Chem., 65, i.
Parravano, N. and de Cesaris, P.
(1912) Att accad.Lincei, [5], 2X, I,
535.
(1912a) Atti accad.Lincei, [5], 2Z, I,
800.
(1912b) Gazz.chim.ital., 42, II, i-
191.
Parravano, N. and Fomaini, 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.
(191 1) J.Am.Chem.Soc., 33, 1933.
Partheil and Ferie.
(1903) Archiv.Pharm., 241, 554.
Partheil and Hfibner.
(1903) Archiv.Pharm., 241, 413.
Partington, J. R.
(191 1) J.Chem.Soc.(Lond.), 99, 315.
Pascal, P.
(1909) Ann.chim.phys., [8], 16, 374.
(1912) Bull.soc.chiin., [4], 11, 323,
596, 1033.
(191 3) Bull.soc.chim., (4I, 13, 746.
(1914) Bull.soc.chim., [ij, 15, 454.
Pascal, P. and Normand, L.
(1913) Bull.soc.chim., [4J, 13, 154-
202, 879.
Patemo, E. and Ampola, G.
(1897) Gazz.chim.ital., 27, I, 481-
556.
Patemo. £. and Miell, A.
(1907) Atti accad.Lincei, [5], 16, II,
153.
(1907) Gazz.chim.ital., 37, II, 330.
Patemo, E. and Salimei, G.
(191 3) 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, iii.
(1896) Z.physik.Chem., 25, 95.
(1901) Arch.Pharm., 239, 64.
(1915) Z.Elektrochem., 21, 543.
(191 7) Z.Elektrochem., 23, 65-86.
Paul, Th., Ohlmiiller, W., Heise, R.
and Auerbach, Fr.
(1906) Arb.Kaiserl.Gesundheitsamt.,
23i 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 FUemonowicz.
(1888) Ber., 21, 2973.
Payen.
(1852) Compt.rend., 34, 356.
Pearce, J. If. and Fry, E. J.
(1914) J.Phys.Chem., 18, 667.
Pearce, J. If. and Moore, T. E.
(1Q13) 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., 245, 118.
Pelabon.
(1908) Compt.rend., 146, 975.
(1909) Ann.chim.phys. [8], 17, 52^-
66.
(191 3) Compt.rend., 156, 705-7.
Pelet-Jotivet
(1909) Revue gen. mat. col., p. 249.
Pellini, G.
(1906) Gazz.chim.ital., 36, II, 461.
(1906a) Atti accad.Lincei, [5I, 15, I,
629.
(1909) Atti accad.Lincei, [5], 18, I,
703; II, 21, 280.
(19 10) 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, [5I, 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) f.Chem.Soc.(Lond.), 81, 480.
(1903) J.Chem.Soc.(Lond.), 83, 1168.
Pettersson, O. and Sond^n, K.
(1889) Ber., 22, 1439.
Pfannl, M.
(191 1) Monatsh.Chem., 32, 250.
Pfaundler and Schnegg.
(1875) Sitzber.k.Akad.Wis.(Wien).,
7I1 II, 351.
Pf eiffer, 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 Wiirgler.
(1 91 5) Ber., 48, 1939.
(1916) 2^physiol.Chem., 07, 128-47.
Phelps, I. El. and Palmer, H. E.
(1917) J.Am.Chem.Soc., 39, 140.
Philip, James C.
(1903) J.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 Gamer, F. B.
(1909) J.Chem.Soc.(Lond.), 95,
1466-73.
810
AUTHOR INDEX
Philip, J. C. and Smith, S. H.
(1905) J.Chem.Soc.(Lond.)» 87,
1735-1751.
Pickering, S. U.
(1890) J.Chem.Soc.(Lond.), 57, 331.
(1890-^1) Proc.Roy.Soc.(Lond.), 49»
25.
(1893) J.Chem.Soc.(Lond.), 63, 141,
463, 909, 998.
(1893a) Ben, 26, 2307.
(1895) J.Chem.Soc.(Lond.), 67, 669.
(1912) Landolt and Bdrnstein,
" Tabellen," 4th Ed., p. 471.
(1915) J.Chem.Soc.(Lond.)i 107,
942-54.
Pictet, Raoul.
(1894) Compt.rend., 119, 642.
Pictet, R. and Altschtd, M.
(1895) Z.physik.Chem., 16, J 8.
(1894) Compt.rend., 119, 678-82.
Pierre.
(1847) J.pharm.chim., [3], 12, 237.
Pina de Rubies, S.
(1913) Anales soc.espan.fis.quin., 11,
422-35.
(19 1 4) Anales soc.espan.fis.quin., 12,
(19 1 4) Archiv.sci. physique, naturelle
(Madrid), [4], 38, 414-22.
(191 5) Chem.Zentralbl., I, 521.
Pinnow, J.
(191 1) 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.
(191 1) Ann.inst.Polytech.Kiev., 11,
310.
(191 5) J.Russ.Phys.Chem.Soc., 47,
1062-4.
Poggiale.
(1843) Ann.chim.phys., [3I, 8, 467.
Pohl.
(1852) J.prakt.Chem., 56, 216.
(i860) Sitzber.k.Akad.Wiss.(Wien),
41, 627.
PoUacd.
(1896) L'Orosi, 19, 217.
Pollitzer, F.
(1909) Z.anorg.Chem., 64, 121-48.
Poma, G.
(1909) Atti accad.Lincei, [5I, 18, I,
133-8.
(1910) Gazz.chim.ital., 40, I, 197.
Poma, G. and Gabbi, G.
(1912) Gazz.chim.ital., 42, II, 8.
(191 1 ) Atti accad.Lincei, [5], 20, I,
464-70.
81
Porlezza, C.
(1914) Atti accad.Lincei, [5], 23, II,
509, 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 Tames, C.
(191 1 ) 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 HUpert, W. S.
(1909) J. Am. Med. Assoc., 52, 311.
- Puclmer, W. A. and Warren, L. E.
(1910) Proc.Am.Pharm.A!s80c., 58,
1007.
(1910) Lab.Reports Am. Med. Assoc.,
3i 1 2 J.
Puschin, N. A. and Baskow, A.
(19 1 3) Z.anorg.Chem., 81, 347-63.
Puschin, N. A. and Glagoleva, A. A.
(19 14) Ann.Inst.Eiectrotechnique
(Petrograd), 11, 284.
(1915) J.Russ.Phys.Chem.Soc., 47,
100-13.
Pushin, N. A. and Grebenschikov, L V.
(1913) J.Russ.Phys.Chem.Soc., 45,
741-5.
Pushin, N. and Enger, J.
(19 1 3) Ann.Inst.Eiectrotechnique
(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.Eiectrotechnique
(Petrograd), 10, 205.
Querdgh, E.
(1912) Atti accad.(Lincei), [5], 2X, I,
417, 786.
(1914) Atti accad.(Lincei), [5], 23, I,
449, 825.
Rabe, W. O.
fi90i) Z.physik.Chem., 38, 175-184.
(1902) Z.anorg.Chem., 31, 156.
Rack, G.
(19 14) Centr.Min.Geol., 326-8.
Radan.
(1889) Liebig's Ann.. 251, 129.
AUTHOR INDEX
Raffo, M. and Rossi, G.
(191 5) Gazz.chim.ital., 45, I, 45.
Rammelsberg.
(1838) Pogg.Ann., 43, 665; 44i 575-
(1841) Pogg.Ann., 52, 81, 96.
(1892) J.prakt.Chem., [2], 45, 153.
Ramsted^Evm.
(191 1 ) Radium, 8. 253-6.
Pankin, G. A. and Mcrwin, H. £.
(1916) J.Am.Chem.Soc., 38, 568.
Rankin, G. A. and Wright
(1915) Am.Jour.Sci., [4], 39» 1-79-
Raoult
(1874) Ann.chim., [5], x, 262.
Raupenstranch, G. A.
(1885) Monatsh.Chem., 6, 585.
Rebiere. G.
(1915) Bull.soc.chim., [4], 17, 268,
Regnault and "Wlllejean.
(1887) Chem.Centralbl., 18, 253.
Reich.
(1891) Monatsh.Chem., la, 464.
Reichel, H.
(1Q09) Biochem.Ztschr., aa, 156.
Reicher. L. T. and van Deventer, C. M.
(1890) Z.physik.Chem., 5, 560.
Raid.
(1887-88) Proc.Roy.Soc.(Edin.), 15,
151.
Reid, H. S. and Mcintosh, D.
(1916) J.Am.Chem.Soc., 38, 615-25.
Reinders, W.
(1900) Z.physik.Chem., 3a, 494, 514.
(1906) Z.physik.Chem., 54. 609.
(1914) Proc.k.Akad.Wet.(Amst.),x6,
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.(Am8t.), 15,
474.
Reinders, W. and Lely, Jr. D.
(1912) Proc.k.Akad.Wet.(Am8t.), 15,
486.
Reinitzer, D.
(19 1 3) Z.angew.Chem., 36, 456.
Reissig.
(1863) Liebig's Ann., 127, 33.
Retgers. J. W.
(1893) Z.anorg.Chem., 3, 253, 344.
(1893) Rec.trav.chim., 12, 229.
Rez.
(1906) Z.physik.Chem., 55, 355.
ReVdiler, 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 Ardiibald, £. H.
ri90i-02) Proc.Am.Acad., 37, 345.
(1902} Z.physik.Chem., 40, 385-98.
Richards, T. W. and Charcfaitt.
(1899) Zj)hy5ik.Chem., 28, 314.
Richards, T. W. and Faber, H. B.
(1899) Am.Chem.Tour., 21, 167—172.
Richards, T. W. and Keiley.
(191 1 ) J.Am.Chem.Soc., 33, 847.
Richards, T. W., McCaffrey and Bisbee.
(1901) Z.anorg.Chem., 28, 85.
Richards, T. W. and Meldiiun, 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.phy8ik.Chem., 45, 461.
Riley, w. A.
(191 1) Jour.Inst.Brewing, 17, 124.
(ipii) ^' Tables annuelles," 2, 428.
ibach, E.
;i897) Ber.. 30, 3079.
1902) Ber., 35, 1300.
Rim!
(1007) Z.anore.Chem., 52, 407.
ibach, E. and Schubert, A.
(1000) Z.physilcChem., 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.
(191 1 ) Z.Kryst.Min., 49, 152.
Robertaon, 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 pnifungs-
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) BuU.sci.Pharmacologique, 20,
7.72.
Rohland, P.
(1897) Z.anorg.Chem., 1%^ 412.
(1808) Z.anorg.Chem., x8, 328.
Roloff, M.
^1894) Z.physik.Chem., 13, 341.
(1895) Z.physik.Chem., 17, ^25-^6.
(1895) Z.physik.Chem., i8i, 572-84.
812
AUTHOR INDBX
i!
Roozeboom, H. W. B.
^1884) Rec.trav.chim., 3, 29-57.
(1885) Rec.trav.chim., ^, 69.
'1887) Rectrav.chim., o, 342.
1888) Z.physik.Chein., a, 459, 518.
;i889) Rec.trav.chim., 8, 1-146.
(1890) Z.physik.Chem., 5, 201.
{1891) Z.physik.Chem., 8, 532.
?i89i) Rec.trav.chim., xo, 271.
[1S92) Z.physik.Chem., 10, 477.
[1893) Rec.trav.chim., 12, 205.
;i899) Proc.k.Akad.Wet.{Am8t.), i,
466.
Rosco6«
(1866) J.Chem.Soc.(Lond.). ig, 504.
Roscoe and Dittmar.
(1859) Liebig's Annalen, 112-^34.
Rosenbladt.
(1886) Ber., ig, 2531. ^
Rosenheim, A and Bertheim, A*
(1903) Z.anorg.Chem., 34, 430.
Rosenheim, A. and Davidsohn, L
(1903) Z.anorg.Chem., 37, 315.
Rosenheim, A. and Griinbaum.
(1909) Z.anorg.Chem., 61, 187.
Rosenheim, A and Piitze, 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.), lox,
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.
J912) 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.Rus8.Phys.Chem.Soc., 38,
782.
Rozsa,M.
(191 1 ) Z. Elektrochem, 17, 935.
Rubenbauer.
(1902) Z.anorg.Chem., 30, 334.
Radorff.
(1862) Pogg.Ann., X16, 63.
(1869) Ber., 2, 70.
Riidoiff.
(1872) Pc^.Ann., 145, 608.
(1873) Ber., 6, 482.
(1885) Ber., x8, 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 Hech^ L.
(191 1 ) 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.
(191 1) Z.anorg.Chem., 72, 341.
RuSS, O. and Winterfeid.
(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.
R7d,S.
(191 7) Z.£lektrochem., 23, 19-23.
S.
(1905) Apoth.Ztg., 20, 1031.
Sackur, O.
(191 1-2) Z.physik.Chem., 78, 553-
568.
(1913) Z.physik.Chem., 83, 297-314.
Sackur, O. and Ftitzmaim, E.
(1909) Z.Elektrochem., 15, 842-6.
Sackur, O. and Taegener, W.
(1912) Z.Elektrochem., x8, 722.
Sahmen, R.
(1905-06) Z.physik.Chem., $4, iii-
120.
Sakabe, S.
(1914) Mem.Coll.Sci.(Kyoto), x, 57-
61.
Salkowski, H.
(1885) Ber., x8, 321.
(1901) Ber., 34, 1947.
Salkower, B.
(1916) Am.J.Pharm., 88, 484.
Salzer.
(1886) Liebig's Ann., 232, 114.
Sammet, V.
(1905) Z.phy8ik.Chem., 53, 644-48.
Sander, W.
(1911-12) Z.phy8ik.Chem., 78, 513-
549.
Sandonnini, C.
(191 1) Atti accad.Lincei, [5], 20, I,
173, 253.
!i9ii^ Gazz.chim.ital., 4X, II, 146.
191 1) Atti accad.Lincei, [5], 20, II,
62, 497, 572, 588, 646.
(1911a) Atti accad.Lmcei, [5], 30, I,
457, 760.
813
AUTHOR INDEX
SandomiJiii, C.
(1912) Atti accad.Lincei, [5], 2Z, I,
208-13. 479.
(1912a) Atti accad.Lincei, [5], 21, II,
197, 524, 635.
(1912b) Atti Ist.Ven., 71, 553.
i accad.Linc
630; II, 21.
(19 1 3) Atti accad.Lincei, 15], 22, I,
• 553.
(1914) Atti accad.Lincei, [5], 23, I,
962.
(191 4) Gazz.chini.ital., 44, 1, 296, 382
Sandonnini, C. and Aureggi, P. C.
(1912) Atti accad.Lincei, [5], ai, I,
493.
Sandonnini, C. and Scarpa, G.
(1911a) Atti accad.Lincei, [5], 20, II,
62.
(1911b) Atti accad.Lincei, [5], 20, II,
497.
(1912) Atti accad.Lincei, [5], 21, II,
77-^4.
(1913) Atti accad.Lincei, [5], 22, II,
21, 163, 518.
Sandqnist, H.
(191 1 ) Liebig's Ann., 379, 85.
(19 1 2) Liebig's Ann., 392, 76.
Ark.Kem.Min.GeoL, 4, 8-81.
Saposchinikow, Gelvich et al,
U903) J.Russ.Phys.Chem.Soc., 35,
1073^4.
(1904) Z.physik.Chem., 49, 688-96.
Savorro. EgUe.
(1914} Atti accad.sci. (Torino), 48,
, ^ 948-59.
(19 14) Chem.Abs., 8, 340.
Sborgi, 11.
(1913) Atti accad.Lincei, [5], 22, I,
91. 636, 716, 798.
(1915) Atti accad.Lincei, [5], 24, I,
1225.
Sborgi, 11. and Mecacd, F.
(191 5) Atti accad.Lincei, [5], 24, I,
443-8.
(1916) Atti accad.Lincei, [5], 25, II,
327, 386, 455.
Scaffidi,V.
(1907) Z.phy8ik.Chem., 52, 42.
Scarpa, G.
(1912) Atti accad.Lincei, [5], 21, II,
720.
(191 5) Atti accad.Lincei, [5], 24, I,
741, 955; n, 476.
Scarpa, O.
(1904) J.chim.phys., 2, 449.
Schachner, Paul.
(1910) Biochem.Centralbl., 9, 610.
Schaefer, G. L.
fi9io) Am.Jour.Pharm., 82, 175.
(19 10) Pharm.Jour.(Lond.), 84, 757.
(1912) Am.Jour.Pharm., 84, 389.
(191 3) Am.Jour.Pharm., 85, 441.
SdiMf er. H.
(1905) Z.anorg.Chem., 45, 310.
Schaefer, W.
(1914) Neues Jahrb.Min.GeoL, 1, 15-
24.
▼on Sdi6ele, C.
(1899) Ber., 32, 415.
Scheffer, F. E. C.
(1911) Proc.k.Akad.Wet.(Amst.), 13,
829; 14, 195.
^1912) Z.physik.Chem., 76, i6i.
(1912a) Proc.k.Akad.Wet.(Amst.),
i5f 380.
Scheibler, C.
{1872) Ber., 5, 343.
(188: -
814
[883) J.pharm.chim., [5 J, 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., 7a, 5^5-35-
Schiavor, G.
(1902) Gazz.chim.itaL, 32, II, 532.
Schick, K.
(1903) Z.physik.Chem., 42, 163.
Schierholz.
(1890) Sitzber.k.Akad.Wiss.(Wien.),
zoz, 2&, 4.
SchifF.
^1859) Liebig's Ann., 109, 326.
(i860) Liebig's Ann., 113, 350.
(1861) Liebig's Ann., 118, 365.
Schiff and Monsacchi.
(1896) Z.physik.Chem., ai, 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.
Schdne.
(1873) Ber., 6, 1224.
SchSnfeld.
(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.
AUTHOR INDEX
SchreinemakerSi F. A. H.
(1898) Zj)hy8ik.Chem., 26, 237-54.
(1898c) Z.phy8ik.Chem., 27, 95-122.
(1899) Z.phy8ik.Chem., 29, 577.
(1900) Proc.k.Akad.Wet.(Amst.), 2,
I.
(1900) Z.physik.Chem., 33, 79.
(1903) Z.anor^.Chem., 37, 207.
1906) Z.physik.Chem., 55, 89. .
1907) Z.physik.Chem., 59, 641.
I1908-09) Z.physik.Chem., 65, 555,
575.
[1908) Chem.Weekblad., 5, 847.
1909) Z.physik.Chem., 66, 687-98.
1909) Chem.Weekblad., 6, iii, 140.
,1909-10) Z.phy8ik.Chem., 68, 83-
103.
(1910) Arch.neer.sc.ex.nat., [2], 15,
81, 117.
'1910) Zj)hy8ik.Chem., 69, 557-68.
1910a) ^.physik.Chem., 71, 109-16.
J9iob) Chem.Weekblad., 7, 333.
(191 1 ) ProcJc.Akad.Wet.(Amst.), 13,
1 163.
Schreinemakers, F. A. H. and de Baat,
W. C.
^1908) Chem.WeekbL, 5, 465-72.
(1908-9) Z.physik.Chem., 65, 586.
!I909) Z.physik.Chem., 67, 551-60.
1910) Chem.Weekblad., 7, 259.
(1910a) Arch.neer.sc.ex.nat., [2], 15,
415.
(1914) Proc.k.Akad.Wet.(Amst.), 17,
533. 781-
(1915) Proc.k.Akad.Wet.(Amst.), 17,
iiii.
(1915) Verslag.k.Akad.Wet.(Amst.),
23» 1097; May.
(1917) Chem.Weekblad., 14, 141,
203, 24A.
(191 7) Chem. Weekblad., 14, 262-7,
288.
Schreinemakers, F.A^. 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.
SchreinenuJcers, 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.
(191 1) 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.
i
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.
(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., 11, 449.
Schroeder, J.
(1905) ^.anorg.Chem., 44, 6.
(1908) J.prakt.Chem., [2], 77, 267-8.
SchlUcarew, A.
(1901) Z.phy8ik.Chem., 38, 543.
Schtdcow.
(1900) Z.Ver.Zuckerind, 50, 313.
Schiller.
(1879) Sitzb.k.Akad.Wis. (Berlin), 79,
302.
Schultz.
(i860) Zeit.Chem., [2], 5, 531.
(1861) Pogg.Ann., 113, 137.
Schulze.
(1881) J.prakt.Chem., [2], 24, 168.
Schweissanger.
(1884-85) Pharm.Ztg.
Schweitzer.
(1890) Z.anal.Chem., 29, 414.
Schwicker.
(1889) Ben, 22, 1731.
Sedlitzt^.
(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.,
(1909) J.Am.Chem.Soc., 31, 1164.
(1910) Bull.N0.67 Hygienic Labora-
tory, U. S. Public Health
' Service.
(1910a) Proc. Am. Pharm. Assoc., 58,
1031.
(1912) Am.Chem.Jour., 48, 453-67.
Seidell, A. and Smith, J. G.
(1904) J.Phy8.Chem., 8, 493.
815
AUTHOR INDEX
Sell, P. A. W. cad GfoenUb, H. G.
(1907) Pharm.Jour.(Lond.), 78, 327.
Seliwanow, Th.
(1914) Z.anorg.Chem., 85, 337-
Sehiud, J.
(1909) Compt.rend.y 148, 1394.
SerulUs.
( ) AniLchim.phyB.» 22f 118.
Sestini.
(1890) Ga2z.chiin.ital.» ao, 313.
Setachenow.
(1892) Ann.chim.phys., [6], 25, 226.
Setterbttrg.
(1882) Liebig's Annahii, azi^ 104.
Seubert and mten.
(1892) Z.anorB.Chem., 2, 434.
Sevier, C. A.
(1908) Analyst. 33, 454-7-
Sevier, C. A. and Lloyd, P. V.
(1909) J.Chem.Soc.(Lond.), 95,1347-
52-
Shad, K. and Bomemann, K.
(1916) Metall u.Erz., 13, 251-62.
Sharwoodj W. J.
(1903) J.Am.Chem.Soc., 25, 576.
Sherrill, M. S.
(1903) Z.phy8ik.Cheni., 43, 705-740.
Shenill, M. S. and Eaton, F. M.
(1907) J.Am.Chem.Soc., 29, 1643.
Sherrill, M. S. and Ruas, D. £.
(1907) J.Am.Chem.Soc., 29, 1657-61.
Shiomi, T.
(1908) Mem.Coll.Sci.Eng. (Kyoto), z,
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 ^Tils-
don, B. H.
(191 1) J.Chem.Soc.(Lond.),99,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, annueiles." 3, 337.
Sieverts, A. and Co-wotkitn.
(1909) Ber., 42, 338.
(1910) Ber., 43, 893.
(1912) Ber.. 45, 221.
Sieverta, A and Bergner, E.
(1912) Ber.. 45» 2576.
Sill, H. F.
(1905) Z.physik.Chem., 51. 577-602.
(191 6) J.AnLChem.Soc.. 38, 2632.
Sims.
(1861) Liebig'a Ann., zi8, 340.
Stnnige, L. R.
(1909) Z.phy8ik.Chem., 67, 432-45.
^ P-
(1902) BulLsocchiiB.. [3]. 27, 905.
Skizrow^ F. W.
(1902) Z.physik.Chem.. 4Z, 144.
Skinner, S.
(1892) J.Chem.Soc(LQnd.). 61, 342.
Skosaareswliy, M. and Tchitehiaadze,
N.
(1916) T.chim.phys., Z4, Z53-r75.
SkrabaL A.
(191 7) Monatsh.Chem.. 38, 25-9.
SUde, R. S.
(19 1 2) Z.ElecktrochenL. z8, i.
Sloan and Mallet
(1882) Chem.News.. 46, 194.
Slotfaouwer, J. EL
(1914) Rec.trav.chim., 33, 327.
Sfiiim<^, WladinLw.
(1907) Z.phyaik.Chem.. 58, 373. 667.
Smith.
(191 2) Landolt and Bdmstetn *' Tab-
ellen.'* 4th Ed., p. 481.
Smith and Bradbury.
(1891) Ber.. 24, 2930.
Smith. A. and Carson, C. M.
(1908) Z.physik.Chem., 6z, 200.
Smith, A. and Eastlack, H. B.
(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 Menziea, A. W. C.
(1909) J.Am.Chem.Soc., 3Z, 1 183-91.
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.
Smitii, Herbert, J.
(191 8) J.Am.Chem.Soc., 40, 879-885.
Smia^ W. R.
(1909) J.Am.Chem.Soc. 3Z, 245.
Smits, A.
(1903) Z.Elecktrochem. 9, 663.
Smits, A. and Bokhorst, S. C.
(191 5) Z.physik.Chem., 89, 374.
Smits, A. and Kettner, A.
(1912) Proc.k.Akad.Wet.(Amst.). Z5,
685.
Smits, A and de Leeuw, H. L.
(1910) Proc.k.Akad.Wet.(Amst.). Z3,
329.
Smits, A and Maarse, J.
(191 1) Proc.k.Akad.Wet.(Amst.). Z4,
192.
Smits, A. and de Mooy.
(1910) Verslag.Akad.W«t.(Amst.),
i^ 293.
816
AUTHOR INDEX
Smits, A. and PostnuL S.
(1914) Proc.k.Akad.Wet.(Am8t.)> i7>
183.
Smolensky, S.
(1911-12) Z.anorg.Chem., 73f 293.
Sneider.
(1866) Pogg.Ann., I27» 624.
Snell, J. F.
(1898) J.Phys.Chein., 2, 474, 484.
Snyder.
(1878) Ber., II, 936.
Soch, C. A.
(1898) J.Phys.Chefn., 2, 43.
Sommer, F.
(19 14) Z.anorg.Chem., 86, 8^.
Sosman, R. B. and Memin, H. £.
(19 1 6) J.Wash.Acad.Sci., 6, 532-537.
Sottdiay and Leussen.
(1856) Liebig's Ann., 99, 33.
Spencer, J. F.
(1912) 2.physik.Chem., 80, 701.
(1913) Z.physik.Chem., 83, 293.
Spencer and LePla.
(1909) Z.anorg.CMein., 65, 14.
Speyers, C. L.
(1002) Am.J.Sci., [4], 14, 294.
Spielrein, C.
(191 3) Compt.rend., 157, 46.
Spring and Ronmanoff .
(1896) Z.anorg.Chem., I3f 34*
Squire, P. W. and Caines, C. M.
(1905) Pharm.Jour.(Lond.), 74, 720,
784.
T. Stackelberg, £. F.
(1896) Z.physik.Chem., 20, 337-58.
van der Stadt, £.
(1902) Z.physik.Chem., 41, 353.
Stanley, H.
(1904) Chem.News, 89, 193.
Stark, G.
(191 1 ) Z.anorg.Chein., 70, 174.
Steger.
(1903) Z.phy8ik.Chem., 43, 595.
Stem, 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.
(19 1 3) J.Russ.Phys.Chem.Soc., 45,
912-30.
Steele and Johnson.
(1904) J.Chem.Soc.(Lond.), 85, 116.
Steiner, P.
(1894) Ann.der.Physik.(Wiedennan),
5a»275.
Steinwehr.
(1902) Ann.der Physik.(Drude), [4],
9» 1050.
Stepanow, A.
(1907) Z.ge8.Schiess,u.SprengstofFw.,
3,43-^.
Stepano, A.
(19 10) J.Russ.Phy8.Cbeni.Soc., 42,
489.
(1910) Liebig's Ann., 373, 219.
Stiassny.
(1891) Monatsh.Chem., I2» 601.
Stich, C.
(1903) Pharm.Ztg., 48,
(1003) Phann.Jour.(Lon<
Stock, A.
, 70, 700.
(1904) Ber., 37, 1432.
(loio) Ber., -J3, 156, 1227.
Stock, A. and &uss, £.
(1917) Ber., 50, 159-164.
Stoermer, R. and Heymann, P.
(1913) Ber., 46, 1255.
Stolba.
1 1 865) J.prakt.Chem., 94, 406.
^1867) J.prakt.Chem.., loi, i.
1872) Z.anal.Chem., 11, 199.
,1877) Chem.Centralbl, 418, 578.
(1883) Chem.Centralbl., 293.
(1889) Chem.Techn.Cent., Anz., 7,
« « ^59.
StoUe.
(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, 11.
(1897) Z.physik.Chem., 22, 62.
^1900) Z.physik.Chem., 34, 109.
(1902) Rec.trav.chim., 2X, 407.
(1907) Rec.trav.chim., 26, 245.
Straub, Jan.
(1911) Z.physik.Chem., 77, 332.
Str6mholm, D.
ri90o) Ber., 3J. 835.
(1903) Z.physik.Chem., 44, 721-32.
(1908) Z.anorg.Chem., 57, 72-103.
Stmve.
(1870) Z.anal.Chem., 9. 34.
(1899) J.prakt.Chem., [2], 61, 457.
Sudborough, J. J. and Lakhnmalanl,
(1917) J.Chem.Soc.(Lond.), xii, 44.
Sudhaus, Kftthe.
(1914) Neues Tahrb.Min.Geol.(Beil.
Bd.), 37, 1-50.
Sole.
(1900) Z.anorg.Chem., 25, 401.
S&s, J.
(191 3) 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).
ri9ii) J.Am.Cbem.Soc., 33, 1814*
817
AUTHOR INDEX
Swione, R.
(1013) Z.physik.Chem., 84, 348.
SzatnmiLry de SzadunAr, L. ▼. '
(1910) Z.Farb.Ind., 7, 215.
. (1910) Chem.Abs., 4, 1381.
de Szjrszkowskif Bohdan.
(19 1 5) Medd.K.Vetenskapsakad,No-
belinst., 3, Nos. 3, 4, 5.
Taber, W. C.
(1906) J.Phy8.Chem., 10, 595.
(1906) Bull., 33, Bureau of boils, U. S.
Dept. Agr.
Taf el, J.
(1901) Bcr., 34, 263.
Takenclii, J.
(1915) Mem.ColLSci.(Kyoto), 1,249-
Taiiim,0.
(1910) Z.physik.Chem., 74, 499.
Tanigi, N.
(1904) Gazz.chini.ital., 34, I, 329.
(1914) Gazz.chim.ital., 44, I, 131.
Tanigi, N. and Checchi. Q.
(1901) Gazz.chim.ital., 31, II, 439.
445-
Taveme, H. J.
(1900) Rec.trav.chim., 19, 109.
Tavlor, H. S. and Henderson, W. N.
(1915) J.Am.Chem.Soc., 37, 1692.
Tavlor, S. F.
(1897) J.Phy8.Chem., i, 301, 468,
720.
Tcherniac, J.
(1916) J.Chem.Soc.(Lond.), 109,1239.
Tetta Polak van der Goot.
(19 13) 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 Cumming, Alex. C.
(1915) J.Chem.Soc.(Lond.), X07,
361-6.
Thomas.
(1896) Compt.rend., 123, 943.
Thomas, T. S. and Risle, A.
(1917) J.Cheni.Soc.(Lond.), iii,
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.),
22, 570-2.
Thorin, E. 6.
(191 5) Z.physik.Chem., 89, 687.
Tichomirow, W.
(1907) J.Russ.Phy8.Chem.Soc., 39,
731-43-
(1908) Chem.Zentralbl., I, 11.
Tllden, W. A.
(1884) J.Chem.Soc(LoiKL). 45, 269,
409.
Tnden and Shenstone.
(1883) ProcRoy.Soc.(Lond.), 35, 345
(1884) PhiLTrans., 23-31.
{1885) Proc Roy. See (LoocL), 38,
331.
Timof eiewp wladimir.
(1890) Z.physik.Chem., 6, 147.
(1891) Compt.rend., 112, 1137, 1224.
(189^) Dissertation (Kharkhov.)
Timof eiew and Kravtzor.
(1915) Chem.Ab8., 9, 2896.
(191 7) Chem.Abs., xi, 788.
TImmennans, J.
(1907) Z.physilcChem., 58, 129-213.
(1910) Proc.k.Akad.Wet.(Amst.) 13,
523-
(191 1 ) " Recherches expenmentales
sur les phenom^nes de
demixtion des melanges
liauides " (Th^se) Bnix-
etfes. Avril, 191 1.
(1912) BuIl.soc.chim.(Belg.), 26, 382.
Tinkler, C. K.
(i9i3)J.Chem.Soc.(Lx>nd.), 103, 2176.
TitherbY, A. W.
(1912) Pharm.Jour.(Lond.), 8S, 94.
Tobler.
(1855) Liebig's Ann., 95, 193.
Tower.
(1906) Z.anorg.Chem., 50, 382.
Traube.
(1884) Ber., 17, 2304.
Traube, L
(1909) Ber., 42, 2185, 4185-8.
Trautz and Anschiitz.
(1906) Z.physik.Chem., 56, 238.
Treadwell and Renter.
(1898) Z.anorg.Chem., 17, 185.
Treis, K.
(i9i4)Neues.Jahr.Min.(Beil.Bd.)^7,
766-818.
Trevor.
(1891) Z.physik.Chem., 7, 470.
Truthe, W.
(i9i2)Z.anorg.Chem., 76, 129-173.
Tsakalotos, D. B.
(1909) Bull.soc.chim., [4], 5, 397-409.
(1910) Tcur.chim.phys., 8, 343.
(1912) Bull.socchim., [4], 11, 287.
(191 3) Bull.socchim., (4], 13, 282.
(1914) J.chim.phys., 12, 461-3.
Tsakisdotos, D. B. 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 KiltinoYic, S. S.
(1916) J.Chem.Soc.(Lond.) xoo. 1286.
Tttchscliinidt, C. and Follenius, O.
(1871) Ber., 4, 583.
818
AUTHOR INDEX
Turnery W. E. S. and Bissett, C. C.
(1913) J.Chem.Soc.(Lond.),i03|i904.
Tutton, A. E. H«
(1897) J.Chem.Soc.(Lond.)i 7ij 850,
(1907) Proc.Roy.Soc.(Lond.), 79,
(A) 351-82.
Tyrer, Dan.
(1910) Jour.Chem.Soc.(Lond.)» 1>7>
1778-1788.
(1910a) Jour.Chem.Soc.(Lond.), 97i
621-632.
(191 1) Proc.Chem.Soc.(Lond.)f 37»
142.
UhUg, J.
(1913) Centr.Min.Gebl., 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.Phy8.Chem.Soc., 45,
1099.
u. s. P., vnL
(1907) U. S. Pharmacopoeia, 8th,
* decennial revision.
Usher, F. L.
ii9o8) Z.physik.Chem., 62. 622-5.
19 10) J.Chem.Soc.(Lond.5, 97, 66-
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.),
Valeur, A
(1917) Compt.rend., 164, 818-20.
Van de Moer, J.
(1891) Rec.trav.chim., 10, 47.
Vandevelde, A. J. J.
Lsocchim.
Van Eyk, C.
(191 1 ) Bull.
(Belg.), 25,210.
81899) 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.
(191 7) 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.), X05,
1491-1503.
Van't Hoff see van't Hoff .
Van Wyk, H. J.
(1902) Z.anorg.Chem., 3a, 115.
(1905) Z.anorg.Chem., 47, 1-52.
Varenne and Patdeau.
(1881) Compt.rend., 93, 1016.
Vasiliev, A. M. (Wasilieff).
(1909) J.Russ.Phys.Chem.Soc., 41,
N , 748-53; 953-7.
(1910) J.Russ.Phys.Chem.Soc., 42,
423, 562-81.
(1910) Chem.Zentralbl.,II, 1527.
(1910) " Tables annuelles,'* i, 381.
(191 1) 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.
(191 2) 8th Inter.Congr.Appl.Chem.,
2, 238, 255.
Vezes, M. and Mouline, M.
(1904) Bull.soc.chim., [3], 31, 1043.
(i 905-06) Proc. verb.soc.phys.nat.
(Bordeaux), 123.
ViaU, F.
(1914) Bull.soc.chim., [4], 15, 5.
Vignon, Leo.
(1891) Bull.soc.chim., [3I, 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, 1 180.
Vortisch, E.
(1914) Neues Tahrb.Min.Geol.(Beil.
Bd.), 38, 185-272.
(1914a) Neues Tahrb.Mm.Geol.(Beil.
Bd.), 38, 513-24.
Vulpius.
(1893) Pharm.Centralh., 34, 117.
de Waal, A. J. C.
(19 10) Dissertation, Leyden.
(1910) " Tables annuelles."
819
AUTHOR INDEX
WaddeO, JohiL
(1898) J.Phy8.Chem., 2, 336.
(1899) l.Phys.Chein., 3, 160.
(1900) J.Phys.Chem., 4. 161.
Waentif, P. and McXntoah, D.
(1916) Trans. Roy .Soc. (Canada), 9»
'203-9.
(1867) Z.anal.ChenL, 6^ 167.
Wagner. C. L.
(1910) Z.physik.Chem., 71. 430.
Wagner. K. L. and Zemer* a.
(191 1) Monatsh.Chem., 31, 833.
Wagemmann, K.
(191 2) Metallurgie, g, 518, 537.
Walden. P. T.
(1905) Am.Chem.Tour., 34, 149.
(1906) Z^physilcChem., 55, 712.
Walden, P. T. and Centnerszwer, M.
(1902-03) Z.phy8ik.Chem., 42, 454.
Walker, J.
(1890) Z.physik.Chem., 5, 195.
"^. A.
{Walker, J. and Fyffe, W.
(1903) J.Chem.Soc.(Lond.)i 83f 179.
Walker, J. and Wood, J. K.
(1898) J.Chem.Soc.(Lond.), 73» 620.
WaUace.
(1855) J.Chem.Soc.(Lond.)t 7i 80.
Wallace.
(1909) Z.anorg.Chem., 631 i.
Waller, A. D.
(1904-05) Proc.Roy.Soc.(Lond.)f 74»
Walton, J
. H. Jr.,
and Jttddf 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.
Washlmrn, E. w. and Maclnnes.
{191 1 ) Z.Elektrochem., 17, 503.
Washburn, E. W. and Read, J. W.
(1915) Proc.Nat.Acad.Sci.(U. S. A),
I. 191-5-
Wasilieif (see Vasiliev).
Wedekind, E. and Pasdike, F.
(1910) Z.physik.Chem., 73, 127.
Wegscheider, R.
(1907) Liebig's Ann., 351, 87.
Wegscheider, R. and Walten H.
^1905) Monatsh.Chem., 26, 685.
(1907) Monat8h.Chem., 28, 633-72.
Weigel, O.
(1906) Nachr.kgl.Ges.Gottingen, p.
525-48-
(1907) Z.phy8ik.Chem., 58, 293-300.
Weiller, P.
(191 1) Chem.Ztg., 35, 1063-5.
▼on Weimam, P. P.
(191 1) Z.phy8ik.ChenL, 76, 218.
Weiaberg*
(1896) Bull.soc.chira., (3], 15, 1097.
WeUa, H. L.
(1892) Am.Jour.Sci., [3], 44, 221.
Wells, H. L. and Wheeler, EL L.
(1892) Am.Jour.Sci., I3I, 43, 475.
Wells, R.C.
(1915) T.Wa8h.Acad.Sci., 5, 617-22.
(1915) J.Am.Chem.Soc., 37, 1704-
Welk, R. C. and McAdain, D. J., Jr.
(1907) J.Am.Chem.Soc,, 29, 721—7.
Welsh, T. W. B. and Broderscm, H. J.
(1915) J.Am.Chem.Soc., 37, 816.
Wempe. G.
(1912) Z.anorg.Chem., 78, 298-337.
Wenger.
(1892) Am.Chem.Jour., 16, 466.
Wenger. Paul.
(191 1 ) Dissertation, Geneve.
(191 1) '* Tables annuelles," 2, 411.
Wentzel.
( ) Dammer's '* Handbucb.'' 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.
(19 14) Pharm.Weekblad, 51, 1443-6.
Wheeler, H. L.
(1892) Am.J.Sci., [3], 44, 123.
(1893) Am.J.Sci., 3I. 45. 267.
(1893a) Z.anorg.Chem., 3, 432.
Wherry. E. T. and Tanov^, E.
(191 8) 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.Chcm.Soc., 25, 78.
Wibaut, J. P.
(1909) Chemisch >yeekblad, 6, 401.
(19 1 3) Rec.trav.chim., 32, 269.
Wigand, A.
(1910) Z.physik.Chem., 75, 235.
Wildeman.
(1893) Z.phy8ik.Chem., zi, 42^1.
Willstaetter.
(1904) Ber., 37, 3753.
Wilsmore.
(1900) Z.phy8ik.Chem., 35, 305.
Wingard, A.
(19 1 7) Svensk.Fann.Tid8krift, 2X,
289-93.
(1917) Chem.Abs., zi, 2748.
Winkler, L. W.
(1887) J.prakt.Chcm., [2], 34t ^77;
36, 177.
(1891) Ber., 24, 3609.
(1899) Chem.Ztg., 23, 687.
(1901) Ber., 34f I409. I43l.
820
AUTHOR INDEX
l^inkler, L. W.
(1905) Landolt and BSrnstein " Tab-
ellen," 3rd Ed., p. 604.
C1906) Z.physik.Chem., 55, 350.
(1912) Landoit and Bornstein '* Tab-
ellen," 4th Ed., p. 597, 601.
Winteler, F.
(1900) Z.Elektrochem., 7, 360.
'Winterstein, B.
(1909) Arch.exp.Path.u.Pharm,, 62,
14.
Wirth, F.
(1908) Z.anorg.Chem., 58, 219.
(1912) Z.anorg.Chem., 76, 174-200,
( 1 912-13) Z.anorg.Chem., 79, 357.
(1914) Z.anorg.Chem., 87, 1-12.
Wirfh, F. and Bakke, B.
(191 4) Z.anorg.Chem., 87, 29, 47.
Witt, O. N.
(1915) Ber., 48, 767.
V. Wittorff, N.
(1904) Z.anorg.Chem., 41, 83.
Wolnnann.
(1897) Oster.Ung.Z.Zuckerind., 25,
997.
Welters.
(1910) N.Jahrb.Min.Geol.(Beil.Bd.),
30, 57.
Wood, J. Kerfoot.
(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, 1 71-6.
Worden, £. C.
(1907) J.Soc.Chem.Ind., a6, 452.
Worley, F. P.
(1905) J.Chem.Soc.(Lond.), 87, 1107.
Woudstra, H. W.
(1912) 8th Int.Cong.Appl.Chem., 12,
Wright and Thomson.
(1884-85) Phil. Mag. [5], 17,288; 19, i.
Wright, Thomson and Leon.
(1891) Proc.Roy.Soc.(Lond.),49,i85.
Wroczynski, A. and Guye, P. A.
(1910) J.chim.phy&., 8» 197.
Wroth, B. B. and Reid, 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.
(191 4) Dissertation, ZUrich.
Wutfa, B.
(1902) Ber., 35. 2415.
van Wyk, see Van Wyk.
Wyroubofif, G.
(1869) Arin.chim.phys., [4], i6, 292.
(1901) Bull.soc.cnim., [3], 25, 105,
121.
Tamamoto.
(1908) J.Coll.Sci.(Tokyo). 25, XI.
Toung, S. W.
(1897) J.Am.Chem.Soc., 19, 851.
Toung, S. W. and Burke, W. E.
(1904) J.Am.Chem.Soc., 26, 141 7.
(1906) J.Am,Chem.Soc., 28, 321.
Zaayer, H. G.
(1886) Rec.trav.chim., 5, 316.
Zaharia. A.
(1899) Bul.soc. de scante din Bu-
curesci (Roumania), 8,
53-61.
Zalai, D.
(1910) Gy6gyszere8zi Ertesito (Bu-
dapest), 18, 366.
(1910) " Tables annuelles," x, 410.
Zambonini, F. F.
(1913) Atti accad.Lincei, [5], 22, I,
523.
Zawidzki, V.
(1904) Z.physik.Chem., 47, 721.
Zemcznzi^.
(1908) Z.anorg.Chem., 57, 267.
Zemcznzy and Rambach.
(1910) Z.anorg.Chem., 65, 403.
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157-66.
821
SUBJECT INDEX
Acenaphthene, i, 2, 16
bromo, 2
chloro, 2
iodo, 2
Acetaidehvde, 2
phenyl hydrazone, 2
trithio, 732
Acetamide, 2
tribromo, 2
trichloro, 2
Acetanilide, 3, 4
chloro and bromo, 4
nitro, 4, 70
oxymethyl, 13
Acetanisidine, 13
Acetic acid, 5-8, 84, 89, 366, 500, 626
chloro, 5, 9-1 1
cyano, 11
esters, 12
Acetic anhydride, 5
Acetins, mono, di and tri, 13
Acetnaphthalide, 13
Acetone, 13-15. 50, 125, 197, 248, 444.
480,511,525,534.648,695
phenyl hydrazone, 487
Acetphenetidine, 477
Acetophenol, 89
Acetophenone, 9, 10, 16, 84
amino, J^o
Acetotoluidine, 732
Aceturethan, 742
Acetyl acetone, 16
Acetyldiphenylamine, 283
Acetylene. 16, 17. 438
bi iodide, 17
Acetylsalicylic acid, loi. 593
Acetyl tribromophenol, 486
Aconitic acid. 17
Aconitine. 17
Acrylic acid, trichloro. 18
Actmium. 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, 72,
125, 126, 160, 163, 235, 239, 245,
247, 248, 286-294. 296, 298-300,
313, 404-5. 438-9. 466-7, 501, 509-
10, 530, 533, 571 » 574. 628, 636,
671
Alizarin. 20
Allantoin. 20
Allocinnamic acids. 254
Allyl alcohol. 511. 534, 647
isothiocyanic ester. 443
mustard oil. yy
thio urea. 738
Aloin. 20
Alums. 3<>-32, 67. 180, 249. 582. 587,
713.
Aluminium bromide, 21-24
chloride. 25-27
fluoride, 27
hydroxide. 28
oxide, 28, 210
rubidium alum. 582
sulfate. 29. 31
sulfide. 29
thallium alum. 713
Aminopropionic acid. 19
Aminosuccinic acid. 692
Ammonia. 33-38, 70, 43^
Amnionium 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, 41
cerium sulfate, 241. 243
cerium nitrate. 241
chloride, 43. 44-50, 60. 107, 109, 274,
337-8. 353. 6|J3, 75i
chloride carnellite. 48
chloride, ethyl and methyl. 50
chromates, 51
chromium alum. 32
chromium sulfate. 67
citrates. « ^
cobalt chlorides. 256
cobalt malonate. 259
822
SUBJECT INDEX
Ammonium acetate, cobalt sulfate,
copper chloride, 265-6, 270
copper sulfate, 273, 557
didymium nitrate, 281
fluoboride, 51
fiuosilicate, 62
formate, 52
glycyrrhizate, 307
mdium 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, 30
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
sulfoantimonate, 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
Am vl acetate, 12, 70, 71
alcohol, 71, 72
alcohol, ISO, 71, 72, 291
Amylamine, 72
hydrochlonde (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
prooyl, 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
Anthraruhne, 83
Antimony, 83, 705, 712
ammonium sulnde, 69
lithium sulfide, 366, 373
penta chloride, 94
penta fluoride, 94
potassium sulfide, 500-1
potassium tartrate, 96
selenides, 05
sodium sufnde, 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, 06
Apomorphine, hydrochloride, 97, 442
Arabinose, 6piS
Arachidic acid, 97
Arbutin, 97
Ar^on, 97
Anbitol, monobenzal, 698
Arsenic, 58, 705, 712
pentoxide, 100
sulfide (ous), loi
tri bromide, 98
tri chloride, 98
tri iodide, 95, 98
tri oxide, 39, 98-100, 629, 642
Asparagine, 10 1
Asparaginic acid, loi
Aspirin, loi, 593
Astrakanit, 641, 668
Atropine, loi, 102
methyl bromide, 102
Auric, Aurous, (see Gold)
Azelaic acid, 102
Azoanisol, 103
phenetol, 103
Azobenzene, 16, 88, 102, 103, 123, 133,
166
amino, 103
hydroxy, loj
Azobenzoic acid ethyl ester, 103
Azolitmine, 104
Azonaphthalene, 103
Azophenetol, 103, 104
Azotoluene, 103
Azoxyanisol, 103
Azoxybenzene, 103
Azoxybenzoic acid ethyl ester, 103
Azoxyphenetol, 103
Barbituric acid, diethyl, 744
Barium acetate, 104
amyl sulfate, 121, 122
arsenate, 104
benzene sulfonates, 122
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, iii, 509, 557
chlorate, 108
chloride, 45, 99, 108-I11, 643
chroma te, iii, 112
cyanide, 112
ferrocyanide, 112
fluoride, iii, 112
formate, 113
elycerolphosphates, 119
hydroxide, 105, 109, 113, 114
iodate, 114
iodide, 106, iii, 112, 114
iodide mercuric cyanide, 423
lodomercurate, 115
ISO caproate, 107
ISO succinate, 120
laurate, 120
malate, 115
malonate, 115
molybdate, 115
mjrristate, 120
nitrate, 45, 55, 109, 113, 115-7, 166,
.542
nitrite, 117, 118
oxalate, 118, 119
oxide, 106, III, 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. III, 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
Benzaniiide, 124
chloroy 124
Benzaniline, 103
Benzazonaphthalene, 103
Benzene, 2, 5, 9, 10, 21, IT, 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, J, 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, ^
fluoronitro, 85
hexahydro, 280
iodo, 90
isoamyl, 90
mixed halogen substituted, 129, 130
nitro, I, 4, 5, 21, 22, 25, IT, 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, TJ^ 84, 89, 128,
133-145
ammo, 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, anH bromo, 145
Benzoic aldehyde, nitro, 2
anhydride, 145
Benzoin, 103, 124, 133, 145
Benzonitnle, 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 hyaroquinaldine, 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
Benzvl 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, 620-631 (see Sodium tetra,-
borate)
Boric acid, 40, i53-57f 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
Brudne, sulfate, 163
tartrate, 163
Butter fat, 302
Butadiene, diphenyl, 163, 254
Butane, 163
Butyl acetate, 13, 163
alcohol, ISO, 291
alcohols, 164, 165
ammonium percmorate, 44
bromide, iso, 292
chloral, 16^
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, iii, 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, 180
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
alum, fluoride, 27, 183
gold chloride, 181, 308
ydroxide, 183
iodate, 183
iodides, 183-^
iridium chlondes, 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, 18^
tartrate, dihydroxy, 186
telluiacid 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, 18^
bromide mercuric cyanide, 423
butylacetate, 188
butyrates, 190
camphorates, 190
caproate, 190
caprylate, 190 .
carbonate, 19 1-5, 218
chlorate, 196
chloride, 99, iii, 119, 121, 170, 189,
195-202, 641
chloride acetamidate, 198
chloride acetic acidate, 198
chloride alcoholates, X99
chromates, 199
cinnamates, 200
citrate, 200
ethyl acetate, 188
fluoride, 167, 189, 198, 201
formate, 201
glycerophosphate, 201
heptoate, 201
hydroxide, 200-5, 215
iodate, 206
iodide, 198, 201, 206
iodo mercurate, 206
lactate, 206
magnesium chloride, 196
malates, 206-^07
malonate, 207
826
SUBJECT INDEX
Calcium acetate, methyl acetate, i88
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
propj^l 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, 221-2
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 su^ar (see Sugar)
Canthandine, 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
Carmme, 239
Carnallite, 388, 641
Camellite, 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
buty rates, 241
chloride (ous), 242
citrate, 242
cobalticyanide, 242
dimethyl phosphate, 242
double nitrates, 242
double sulfates, 243
fluoride, 242
formate, 241
p^lycolate, 242
lodate, 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, 2^6
caesium sulfate, 186
cerium nitrate, 242
chlorate, 256
chloride, 45, 256-8
citrates, 258
double salts, 255
fluoride, 258
^dolinium nitrate, 304
lodate, 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
CoUidine, 262
Congo red, 262
Coniine, 262
Copiapite, 344
Copper acetate, 262—3
ammonium chloride, 265-^, 270
ammonium sulfate, 27^^ 557
bromide, 167, 263
caesium sulfate, 186
carbonate, 263-4
chlorate, 264
chloride, 109, iii, 150, 264-27a
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
Dibcnzyl, 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,
166, 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, 28J.
Emetine ana 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, 200, 313
Ethyl alcohol (see Alcohol)
amine, di, 128
amine hydrochloride, 296
amine, tri, 102, iii, 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, 4^.2
morphine hydrocnloride, 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, 506, 695-97
Glutaminic acid, 306
hydrochloride, 307
Glutaric acid, 307
Glycerol, 75, 125
Glycine, iii, 307
•Glycocoll, ;jo7
trimethyj, 149
Glycolic acid, 307
phenyl, 307
Glycyrrhizic acid, 307
Gold, 308, 705, 712
caesium chloride, 181
chloride, 308
double chlorides, 308
lithium chloride, 36^
phosphorus trichloride, 308
Grape sugar, 695-97
Guaiacol, 251, 309
carbonate, J09
Guanidine, triphenyl, 2, 309
Gulose, 697
Gun cotton, 465
Helianthin, 309
Helium, J09-310
Hemoglobin, 309
Heptane, 239, 278, 291, 310, 436, 481
Heptoic acid, 310
Heroine, 442
Hexahydrobenzene, 280
Hexamethylene, 280
tetramine, 310
Hexane, 78, 131, 291, 310, 436
Hexanitrodiphenylamine, 283
Hippuric acid, 3 10- 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, beza, 140
Hydrobenzoin, 133
Hydrobromic acid, 15, 160, 248, 313
Hydrochloric acid, 247, 248, 298, 313-S
517. 649 .
Hydrocinnamtc 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
Iodic acid, 325, 536, 654
Iodine, 55, 95, 98, 150, 160, 184, 206,
247, 271. 325-34. 429. 537, 713
lodoeosine, 335
Iodoform, 335
lodol, 335
Iridium ammonium chlorides, 55, 335
caesiuifi 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
Isobutvl 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
lodate, 346
malonate, 346
molybdate, 347
oxalate, 347
sulfate, 348
sulfonates, 348
tartrate, 349
tungstate, 349
Laurie acid, 349
Lead, 349, 705, 712
acetate, 349-35©
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, J57
diphenyl dicydohexyl, 352
double c^^anides, 357
ferricyanide, 357
fluoride, 351. 35^, 357
fluoro chloride, 356
formate, 358
heptylate, 352
hexyl bromide, 352
hexyl chloride, 352
hydroxide, 358
hyposulfate, 365
ioaate, 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, iii, 183, 198, 270, 356,
370-1
chromate, 372
citrate, 372
fluoride, 27, 373
formate, 373
eold chloride, 308, 369
hippurate, 373
hydroxide, 367, 371-3
hypophosphate, 377
icxiate, 374
iodide, 373, 374
iodo 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, 370, 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
ioaate, 390
jodide, 390
iodide alcoholates, 391, 392
iodide anilinates, 391, 392
iodide compounds, 391, 393, 394
Magnesium iodide etherates, 391, 392
icdo mercurate, 394
lanthanum nitrate, 347
laurate, 3^4
mercuric iodide, 394
myristate, 39^
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, 598-400
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, 186
carbonate, 401
cerium nitrate, 242
chloride, 47, in, 170, I98» 35^, 37i»
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
Meilibose, 606
Mellitic acicl, hexamethyl, 431
Menthane, 431
Menthol, 128, i^i, 224, 245, 431
Menthyl mandelates, 400
Mercury, 378, 598
acetate, 406
ammonium iodide, 55
barium iodide, 115
benzoate, 406
bromide, 131, 158, 351 1 406-8
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, ^2, 292
Meta arsenic acid, 98
Methacetin, 13
Methane, 432-3
diphenyl, 86, 92, 433
tnphenyl, 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, 510, 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
carbinoi, tri, 227
chloride, 315, 439
cinnamate, 9, 10
cryptopines, 279
ether, 37, 248, 301, 315, 438
ethyl ketone, 299, 534, 649
hexyl carbinoi, 574
iodide, 436, 439
iso thiocyanate, 443
malonic acid, 399
mellitic acid, nexa, 431
mustard oil, 223
orange, 309, 4J9
oxalate, 439
phenyl carbamide, 226
phenyl picramides, .492
picric acid, 495
piperidines, 496
propionate, A39
propyl azo phenol, 103
pyridines, 574
pyridines, tri, 262
pyridine zinc chloride, 574
salicylate, 251, 439
833
SUBJECT INDEX
Methyl butyrate, succinic acid, 71 1-2
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, 4^7
Naphthoic acids, dihydro, 447
Naphthols, 10, 128, 224, 251, 283, 301,
446, 447, 448, 593, 703,
picrate, 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
ilfate, 186
caesmm sul
Nickel bromate, carbonate, 451
carboxyl, 451
cerium nitrate, 242
chlorate, 451
chloride, 47, 452
citrate, 452
gadolinium nitrate, 304
hydroxide, 452
icxlate, 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, 456-7f 54^
oxide, 418, 461, 465
Nitrocellulose, 465
Nitrogen, 457-461
oxide (ic), 461
oxide (ous), 462-5
tetroxide, 46^
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, 661
Oxybenzoic acids, 140, 141, 251
Oxy benzoic acid, dinitro, 145
Oxygen, 470-3
834
SUBJECT INDEX
Ozokerite paraffin, 475
Ozone, 473-4
Palladium chloride, 474
Palmitic add, 97, 248, 443f 4^7, 474-5»
677
acetic ester, 446
acid cetyl ester, 475
Palmitin, tri, 467, 475
Papaverine, 475
Paraffin, 28^, 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, ij.77
Phenacetm, 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, 146,
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, ^86
amine, di, 21, 80, 128, 282-3
amine, tri, 282
anisyl ketone, 10
benzoate, 10
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
nydracrylic acid, 732
Phenyl hydrazines, 484, 486-7
hydrazme, di, 163
hydrazones of sugars, 697
methane, di, 433
methane, tri, 282, 309, 433-4, 704
methyl amine hydrochloride, 438
methyl carbamide, 226
pipendines, 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, ^87
Phosphomolybdic acid, 488
Phosphoric acid, 224, 489-90
Phosphorus, 488-9
acid, 489
sulfides, 489
triiodide, 95, 98
Phthalic acids, 4^
Phthalic acids, nitro, 491
Phthalic anhydride, 491
Phthalide, 2, 309
carboxylic acid, 492
Phthalimide, 492
Phthalonic acid, 492
Phthalyl hydroxylamine 324
phenyl hydrazides, 312, 487
Physostigmine, 492
salicylate, 492
sulfate, ^92
Phytosterol, 248
Picramides, methyl phenyl, 49?
Picric acid, 5. 81, 240, 279, 301. 303,
309, 446-8, 484, 486, 49^5, 731
methyl, 495
Picrotoxine, 495
Picoline, 574
Pilocarpine, ^96
hydrochloride, 496
mtrate, 496
Pinacolin, 496
Pimelic acid« 495
Pinene, 203
hydrochloride, 496
Pipecoline, 496
Piperidine, 280, 496
propyl, 262
Pipendines, di phenyl 497
Piperidine hydrochloride, 496
methyl, 496
Piperine, 496, 497
Piperonal, 9, 10, 136
nitro, 10
Piperonilic aldehyde, 2
Platinates, chloro, of hydrocarbon sul-
£ne8,499
835
SUBJECT INDEX
Platino amines, 499
Platinous nitrite ammonium com-
pounds, 499
Platinum alloys, 497
ammonium bromide, 41,
bromide, 497
caesium chloride, 182
chlorides, 49^
double chlorides, ^98
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, ^80, 504-7
bromide, mercunc 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, iii, 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, camellite, 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
nippurate, 311
hydroxide, 501, 502, 507. 509, 526,
^ 529. 534-6, 555, 558
hypophosphate, 555
hypophosphite, 555
ioaate, 536
iodide, 100, 177, 326, 425, 504, 505,
507, 518. 519. 526, 534. 536,
537-41
iodide 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
pyrophosphate, 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, 166, 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
Praseodvmium 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, I2, 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
sulnne perchlorate, 698
Pseudo cumidine, 279
Pyrene, 573
Pyridinamino succinic acids, 575
Pyridine, 21, 127, 136, 258, 279, 439,
446, 484, a86, 574
Pyridines, methyl, ethyl, etc., 574
trimethyl, 262
Pyrocatechol, 15, 77, 146, 224, 251,
32A, 446, 575
Pyrogallol, 15, 22^, 575
Pyrone, dimethyl (see Dimethylpy-
rone
Pyrophosphoric acid, 490
Pyrotartaric acid, 307, 71 1-2
Pyroxylin, 465
Suinaldine, benzoyl tetrahydro, 146
uinidlne, 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
Quinhydrone, 575
Quinol, 132, 448
837
SUBJECT INDEX
Quinoline, 484, 486
ethiodide, 579
Radium emanations, 579^80
Rape oil, 468
Rafiinose, 695-97
Resorcinol, 15, 77, 131, 146, 224,
283, 324. 446. 484, 495,
580-1, 654
Retene, IA5
Rhamnitoi, dibenzal, 698
Rhamnose, 696
Rhodium salts, 581
sodium nitrite, 660
Rosolic add, 582
Rosaniline, 581
hydrochloride, 582
Rubidium alum, 32, 582
bicarbonate, 582
bromide, 582
bromiodide, 58^
cadmium bromide, 168
cadmium chloride, 172
caesium nitrosochlonde, 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
pold chloride, 308
lodate, 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, 584
thiocyanate, 567
uranyl chloride, 734
uranyl nitrate, 735
Ruthenium salts, 587
Saccharin, 587-8
Salicin, 588 .
Salicylamide, 588 1
Salicylates, methyl and phenyl, 251 1
Salicylic acid, 15, 136, 251, 480, 575, ;
25i»
575.
588-93
aide
lehyde, 10
Salol, 9, 96, 149, 224, 225, 245, 309»43i.
448. 593
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, ^96
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
SUver, 598, 705, 712
acetate, 598-9, 622
acetyl propionate, 617
arsenate, 600
arsenite, 600
benzoate, 600
borate, 600
bromate, 601
bromide, 351, 367, 507, 582, 601-4
butyrate, 604
caproates, 605
carbonate, 605
chloroacetate, 599-600
chlorate, 605
chloride, 183, 198, 270, 356,37^3*''
583, 604-12
chromate, 612
citrate, 613
cyanide, 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» ^ ^^'
611,615-6
isobutyrate, 604
838
SUBJECT INDEX
Silver, isovalerate, 624
laurate, 617
levulinate, 617
maiate, 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, loi, 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
bisuifate, 670, 672
borate, 367
borate (tetra), 629-31
bromate, 631
bromide, 99, 167, 604-5, 631-2, 634-5
cacodylate, 633
cadmmm 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
cenum 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, 480,
507. 512, 517, 519, 521-2, 526,
544-5, 548. 562, 583, 611, 632, 635,
637, 639-49, 661, 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
ydrogen 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
nitnte, 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. 378r 397, 405, 522, 526,
559, 562, 623, 632, 637, 641, 649,
651-2, 656, 658, 660-1, 667-72,
sulfide, 455, 672
sulfite, 673
sulfoantimonate, 627-^
sulfonates, 673-4
tartrate, 566, 674
tellurates, 674
tetraborate, 367, 629-31
tetracbromate, 650
tetraiodofluorescein, 335
thiocyanate, 567
tbiosulfate, 208, 222, 628, 674-5
thorium sulfate, 725
trichromate, 650
tungsUte, 656, 665, 672, 675
uranyl chromate, 734
uranyl oxalates, 661
urate, 676
yttrium sulfate, 747
zinc sulfate, 75^
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, iii, 119, 170, 198,
356, 371. 388, 526, 649, 679, 680
chromate, 680
cinnamate, 681
fluoride, 680, 681
formate, 681
glycerophosphate, 681
hydroxide, 678, 680-^
byposulfate, 365
iodate, 682
iodide, 682
Strontium acetate, iodide mercuric cy-
anide, 423
iodomercurate, 682
malate, 683
malonate, 683
mercuric, iomde, 682
molybdate, 683
nitrate, 361, 546, 548, 659, 681, 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 add, 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
Sucdnimide, 693
Sucrose (see Sugar)
Sugar, 166, 187, 198, 205, 397. 512,
548, 627, 636, 648, 672, 693-8
Sulfanilic add, 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, 2^.7, 708
"Superphosphates, 212
Syngenite, 218
Tachhydrite, 196, 641
Talitol, tribenzal, 698
Tannic acid, 710
Tantalum ix>tassium 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, 7^0
840
SUBJECT INDEX
Telliirhiin, bromide, diphenyl, 596
caesium chloride, 182
chromium alum, 249
double salts, 712
rubidium chloride, 584
tetra iodide, 713
Terephthalic add, 490
Terpm 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, 1 11, 150, 170, 183, 198, 270,
339» 356t 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,
A46, 465, 478, 729-30
sulfonamines, 729
sulfochloride, 730
trinitro, i, 16, 224, 495, 575
Toluic acids, 9, 10, 12, 136, 575, 730,
Toluidines, 79, 136, 224, 240, 283, 293,
324, 431, 446, 448, 484, 486, 581,
731-2
Tolyl carbamide, 226
Trenalose, 696
Tribenzylamine, 730
Triethylamine, 102, iii (see Ethyl-
amine)
Trimethylamine, 437 (see Methyl-
amines)
Trimethylethylene, 72
Triolein, 467
Trional, 435
Trioxymethylene, 303
Tripalmitin, ^67, 475
Triphenylamine, 282, 732
Triphenyl arsine, 732
Triphenylbismuthiney 732
841
SUBJECT INDEX
Triphenyl phosphine, 732
guanidine, 2
stibene, 732
Tristearin, 467, 475, 677
Trithioacetaidehyde, 732
Trithiobenzaldehyde, 732
Tropaeolin, 309
Tropic acid, 732
Tungsten trioxidei 675
Turpentine, 294, 440, 733
Ulexine, 280
UranyJ 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, 661, 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, 661
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 sulnne 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, 7^.0
caesium sulfate, 186
carbonate, 749
cerium nitrate, 242
chlorate, 750
chloride, iii, 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
Zinc, oxychlorides, 750
phenol sulfonate, 756
potassium cyanidCi 532
pwtassium sulfate, 557
pwtassium vanadate, 568
praseodymium nitrate, 568
rubidium sulfate, 587
saiparium nitrate, 594
silicate, 178, 378
sodium sulfate, 755
Zinc, sulfate, 274-5, 404, 754-5
sulfide, 277, 345, 365, 624, 755
sulfite, 755
sulfonates, 755-6
tartrate, 756
thallium cyanide, 717
thallium sulfate, 720
valerate, 756
Zirconium sodium fluoride, 676
sulfate, 756
843
Table Showing the Volnme Number and Gorreeponding Tear
Clliose journals marked (*) were examined page by page for solubility data. In
last number recorded for each journal is that
1900
Am. Chem. Tour. (*)
Am. Jour. Pharm. (*)
Am. Jour. Sd. (t)
Analyst (t)
Ann. Chem. (Liebig's) (f)
Ann. chim. phys.* (*)
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Ann. Physik (Wed.) (t)
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Chem. Weekblad (♦)
Chem. Ztg
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Elektrochem. Z. (f)
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Intern. Congr. Appl. Chem. (f)
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J. Phys. Chem. {♦)
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J. Rubs. Phys. Chem. Soc
J. Soc. Chem. Ind. (f)
Mem. Coll. Sci. Em. Kyoto* (♦)
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Pharm. Jour. (Lond.) (•)
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23-4
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t Changed to Ann. duxiL in 19x4.
* Changed to Mem. CoU. Sd. (Kyoto) in 19x4.
of Publication of Fifty Chemical and Related Periodicals.
the case of those marked (f), the tables of contents only were searched. Tlie
^* ■■ra«'>' ««
1907
1908
1909
1910
19IZ
1912
1913
1914
191S
1916
1917
37-8
39-40
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45-^
47-8
49-50
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80
81
82
83
84
85
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87
88
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
386^4
395-402
402-4
10-12
13-15
16-18
19-21
22-24
25-27
28-30
1-2
3-4
12
13
14
15
16
17
18
19
20
22-24
25-27
28-30
31-33
34-36
37-40
40-43
43-46
46-48
48-
245
246
247
248
249
250
251
252
253
16
17
18
19
20
21
22
23
24
25
40
41
42
43
44
45
46
47
48
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5
5
6
7
8
9
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5
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17
19
21
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23
24
25
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101-2
103-4
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19-20
20-21
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37
38
39
40
41
42
43
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8th
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38
39
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91
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27
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94-5
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3
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7
8
9
10
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12
13-14
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17-18
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32-33
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79(A)
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86-7(A)
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26
27
28
29
30
31
32
33
34
11-12
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27-28
29-30
31-
46
47
48
49
50
51
52
53
54
20
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
13
14
15
16
17
18
19
20
21
42-4
44-5
46
47
48^
50
51-2
53
57-61
61-65
65^8
68-75
75-78
78-81
81-86
86-89
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59-64
64-70
70-76
77-82
83-88
89-93
93-D5
D. VAN NOSTRAND COMPANY
25 PARK PLACE
NEW YORK
SHORT-TITLE CATALOG
OF
|)nbltcations and Jmportationa
SCIENTIFIC AND ENGINEERING
BOOKS
This list intludcB
the technical publications of the following English pabliihers:
SCOTT, GREENWOOD ft CO. JAMES MONRO ft CO., Ltd.
CONSTABLE&COMPANV.Ltd. TECHNICAL PUBLISHING CO.
BENN BROTHERS, Ltd.
for who.t D. Van Nostrand Compaoyare American agenti.
July, 1919
5H0RT-TITLE CATALOG
OF THE
Publications and Importations
OP
D. VAN NOSTRAND COMPANY
25 PARK PLACE, N. Y.
A.lt f^ice^ in thU IM are ffl^T.
A.ii binding's are tn cloth unless otherwise noted*
Abbott, A. V« The Electrical Transmission of Bner^ Svo, *$5 oo
A Treatise on Fuel. (Science Series No. 9.) lOmo, o 75
Testing Machines. (Science Series No. 74.) i6mo, o 75
Abraham, Herbert. Asphalts and Allied Substances Svo, 5 00
Adam, P. Practical Bookbinding. Trans, by T. £. Haw lamo, *a 50
Adams, H« Theory and Practice in Designing 8vo, *2 50
Adams, H. C. Sewage of Sea Coast Towns 8vo, *2 50
Adams, J. W. Sewers and Drains for Populous Districts 8yo, a 50
Addyman, F. T. Practical X-Ray Work 8vo, 5 00
Adler, A. A. Theory of Engineering Drawing Sto, *2 00
— Principles of Parallel Projecting-line Drawing 8vo, *i 00
Aikman, C. M. ICanures and the Principles of Manuring 8vo, 2 50
Aitken, W. Manual of the Telephone 8vo, *8 qo
d'Albe, E. E. F.,* Contemporary Chemistty lamo, *x 25
Alexander, J. Colloid Chemistry lamo, z 00
Alexander, J. H. Elementary Electrical Engineering i2mo, 250
Allan, W. Strength of Beams Under Transverse Loads. (Science Series
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Theory of Arches. (Science Series No. 11.) i6mo,
Allen, H. Modern Power Gas Producer Practice and Applications. i2mo, *2 50
Anderson, J. W. Prospector's Handbook i2mo, i 50
Andes, L. Vegetable Fats and Oils 8to, "^6 00
Animal Fats and Oils. Trans, by C. Salter Svo, '^'s 00
Drying Oils, Boiled Oil, and Solid and Liquid Driers Svo, ^ 00
Iron Corrosion, Anti- fouling and Anti-coiroaive Paints. Trans, by
C. Salter 8vo, *6 00
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Andrews, £. S., and Hey wood, H. B. The Calculus for Engineers. 12 mo, *2 00
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50
*2
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*2
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2
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2
OQ
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5a
D. VAN NOSTRAND CO/S SHORT TITLE CATALOG 3
Annual Reports on the Progress of Chemistry. Twelve Volumes now
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Argand, M. Imaginary Quantities. Translated from the French by
A. S. Hardy. (Science Series No. 52.) i6mo, o 75
Armstrong, R., and Idell, S. £. Chimneys for Furnaces and Steam Boilers.
(Science Series No. !•) i6mo, o 75
Arnold, £. Armature Windings of Direct-Current Dynamos. Trans, by
F. B. DeGress 8vo, *2 00
Asch, W., and Asch, D. The Silicates in Chemistry and Commerce. 8vo, "^6 00
Ashe, S. W., and Keiley, J. D. Electric Railways. Theoretically and
Practically Treated. Vol. I. Rolling Stock i2mo,
Ashe, S. W. Electric Railways. Vol. 11. Engineering Preliminaries and
Direct Current Sub-Stations i2mo,
Electricity: Experimentally and Practically Applied 12 mo,
Ashley, R. H. Chemical Calculations i2mo,
Atkins, W. Common Battery Telephony Simplified i2mo,
Atkinson, A A Electrical and Magnetic Calculations 8vo,
Atkinson, J. J. Friction of Air in Mines. (Science Series No. 14.) . i6mo,
Atkinson, J. J., and Williams, Jr., E. H. Gases Met with in Coal Mines.
(Science Series No. 13.) x6mo,
Atkinson, P. The Elements of Electric Lighting i2mo,
The Elements of Dynamic Electricity and Magnetism i2mo,
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Aucluncloss, W. S. Link and Valve Motions Simplified 8vo,
Austin, £. Single Phase Electric Railways 4to, *5 oq
Austin and Cohn. Pocketbook of Radiotelegraphy (In Press.)
Ayrton, H. The Electric Arc Syo, 5 5a
Bacon, F. W. Treatise on the Richards Steam-Engine Indicator . . Z2mo,
Bailey, R. D. The Brewers' Analyst 8to,
Baker, A L. Quaternions 8vo,
Thick-Lens Optics i2mo,
Baker, Benj. Pressure of Earthwork. (Science Series No. 56.) . . . i6mo,
Baker, G. S. Ship Form, Resistance and Screw Propulsion 8yo,
Baker, I. 0. Levelling. (Science Series No. 91.) i6mo,
Baker, M. N. Potable Water. (Science Series No. 61.) i6mo,
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Baker, T. T. Telegraphic Transmission of Photographs i2mo,
Bale, G. R. Modem Iron Foundry Practice. i2mo.
Vol. I. Foundry Equipment, Materials Used *3
Ball, J. W. Concrete Structures in Railways 8vo,
Ball, R. S. Popular Guide to the Heavens 8vo,
Natural Sources of Power. (Westminster Series.) 8vo,
Ball, W. y. Law Affecting Engineers 8vo,
Bankson, Lloyd. Slide Valve Diagrams. (Science Series No. 108.)
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Barham, G. B. Development of the Incandescent Electric Lamp . . 8vo,
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0
75
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25
*3
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*2
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*5
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SO
0
75
2
50
2
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Bedell, F., and Pierce, C. A. Direct and Alternating Current Manual.
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BeggSi G. E. Stresaee in Railway Girders and Bridges {In Press,)
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Bernthsen, A. A Text - book of Organic Chemistry. Trans, by G.
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Bersch, J. Manufacture of Mineral and Lake Pigments. Trans, by A. C.
Wright 8vo,
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The Potter's Craft i2mo»
Birchmore, W. H. Interpretation of Gas Analysis x2mo,
Blaine, R. G. The Calculus and Its Applications i2!no, '*'r 75
Blake, W. H. Brewers' Vade Mecum 8vo, *4 00
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5
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5
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0
75
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6
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5
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*4
on
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8
09
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•1
-5
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50
a
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*7 50
7 50
8
50
♦2
50
5
00
5
oa
I
50
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10
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Bottler, M. Modem Bleaching Agents. Trans, by C. Salter. .. .i2mo,
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Bragg, E. M. Marine Engine Design i2mo,
Design of Marine Engines and Auxiliaries Svo,
Brainard, F. R. The Sextant. (Science Series No. loi.) i6mo,
Biassey's Naval Annual for 1915. War Edition Svo,
Briggs, R., and Wolff, A. R. Steam-Heating. (Science Series No.
68.) i6mo.
Bright, C. The Life Story of Sir Charles Tilsoa Bright Svo,
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Brislee, T. J. Introduction to the Study of Fuel. (Outlines of Indus-
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Broadfoot, S. K. Motors: Secondary Batteries. (Installation Manuals
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Broughton, H. H. Electric Cranes and Hoists
Brown, G. Healthy Foundations. (Science Series No. 80.) i6mo,
Brown, H. Irrigation Svo,
Brown, H. Rubber 8vo,
W, A. Portland Cement Industry Svo,
Brown, Wm. N. Dipping, Bumishing, Lacquering and Bronzing
Brass Ware i2mo,
Handbook on Japanning i2mo,
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Brown, Wm. N. The Art of Enamelling on Metal lamo, *2 oo
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Browne, C. L. Fitting and Erecting of Engines 8vo, *i 50
Browne, R. E. Water Meters. (Science Series No. 81) i6mo, o 75
Bruce, £. M. Detection of Common Food Adulterants zamo, z as
Bronner, R. Manufacture of Lubricants, Shoe Polishes and Leather
Dressings. Trans, by C. Salter 8vo, *3 50
Buel, R. H. Safety Valves. (Science Series No. az.) z6mo, o 75
Bunkley, J. W. Military and Naval Recognition Book z6mo, z 00
Burley, 6. W. Lathes. Their Construction and Operation zamo, a 00
Machine and Fitting Shop Practice zamo, a 00
Testing of Machine Tools zamo, a 00
Bumside, W. Bridge Foundations zamo, *2 00
Burstall, F. W. Energy Diagram for Gas. "With Text 8vo, i 50
— Diagram. Sold separately ♦i 00
Burt, W. A. Key to the Solar Compass i6mo, leather, 2 50
Buskett, E. W. Fire Assaying zamo, ♦z as
Butler, H. J. Motor Bodies and Chassis 8vo, '''300
Byers, H, Gi| and Knigbtf H. 0. Notes on Qualitative Analysis — 8vo, *z 50
Cain, W. Brief Course 10 the Calculus i2mo, "^i 75
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Carey, A E., and Oliver, F. W. Tidal Lands 8vo, s 00
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Carter, H. A. Ramie (Rhea), China Grass zamo, *3 00
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Cathcart, W. L. Machine Design. Part I. Fastenings 8vo, *3 00
Cathcart, W. L., and Chaffee, J. I. Elements of Graphic Statics . . .8vo, *3 00
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Chalkley, A. P. Diesel Engines 8vo, "^4 00
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Chambers, G. F. ' Astronomy i6mo, *z 50
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Clausen-Thue, W. A B C Universal Commercial Telegraphic Code.
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Clevenger, S. R. Treatise on the Method of Government Surveying.
i6mo, morocco, 2 50
Clouth, F. Rubber, Gutta-Percha, and Balata Svo, *6 00
Cochran, J. Concrete and Reinforced Concrete Specifications Svo, *2 50
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Cocking, W. C. Calculations for Steel-Frame Structures i2mo, *2 50
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Cole, R. S. Treatise on Photographic Optics z2mo, i 50
Coles-Finch, W. Water, Its Origin and Use Svo, *5 00
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Collins, S. Hoare. Plant Products and Chemical Fertilizers Svo, 3 00
Collis, A. 6. High and Low Tension Switch-Gear Design Svo, *3 50
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Colver, E. D. S. High Explosives Svo, 1250
Comstock, D. F., and Troland, L. T, The Nature of Electricity and
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Coombs, H. A. Gear Teeth. (Science Series No. 120.) i6mo, o 75
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Corfield, W. H. Dwelling Houses. (Science Series No. 50.) i6mo, o 75
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Crais» J. W., and Woodward, W. P. Questions and Answers About
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Wave and Vortex Motion. (Science Series No. 43.) i6mo,
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Creedy, F. Single Phase Commutator Motors 8yo,
Crehore, A. C. Mystery of Matter and Energy 8vo,
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Crosby, E. XJ., Fiske, H. A., and Forster, H. W. Handbook of Fire
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Crosskey, L. R. Elementary Perspective 8vo, i 25
Crosskey, L. R., and Thaw, J. Advanced Perspective Svo, i 50
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Cushing, H. C, Jr., and Harrison, N. Central Station Management ... '''2 00
Dadourian, H. M. Analytical Mechanics i2mo, *3 00
Danby, A. Natural Rock Asphalts and Bitumens 8vo, *2 50
Davenporti C. The Book. (Westminster Series.) 8vo, *2 00
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Denny, G. A. Deep-level Mines of the Rand 4to, *io 00
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Maintenance-of-Way Engineering {In Preparation.)
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Dibdin, W. J. Purification of Sewage and Water 8vo, 6 50
Dichmann, Carl. Basic Open-Hearth Steel Process 12 mo, *3 50
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Franzen, H. Exercises in Gas Analysis i2mo, *i 00
Freudemacher, P. W. Electrical Mining Installations. (Installation
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Friend, J. N. The Chemistry of Linseed Oil i2mo, i 00
Frith, J. Alternating Current Design Svo, ^2 50
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Garrard, C. C. Electric Switch and Controlling Gear 8vo, "^6 00
Gaudard, J. Foundations. (Science Series No. 34.) i6mO| o 75
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Geerligs, H. Cj P. Cane Sugar and Its Manufacture Svo, *6 00
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Gillmore, Gen. Q. A. Roads, Streets, and Pavements z2mo, i 25
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Goodell, J. M. The Location, Construction and Maintenance of
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Goodeve, T. M. Textbook on the Steam-engine i2mo, 2 00
Gore, G. Electrolytic Separation of Metals. . Svo, *3 50
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Grierson, R. Some Modern Methods of Ventilation 8vOy *3 00
Griffiths, A. B. A Treatise on Manures i2mo, 3 00
Dental MeUUurgy 8vo, *3 50
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*7
50
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25
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50
*3
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*2
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Hausner, A. Manufacture of Preserved Foods and Sweetmeats. Trans,
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*9
00
*5
00
*3
50
♦2
50
♦2
50
*3
50
*7
50
*7
50
♦i
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*2
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♦2
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*4
00
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25
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