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Full text of "Solubilities Of Organic Compounds Vol - I"

SOLUBILITIES 

OF 

INORGANIC AND METAL ORGANIC 
COMPOUNDS 



A COMPILATION OF QUANTITATIVE SOLUBILITY 
DATA FROM THE PERIODICAL 
LITERATURE 



BY 

ATHERTON SEIDELL, PH. D. 

National Institute of Health 
Washington, D. C. 



THIRD EDITION 

Vol ume I 




940 



NEW YORK 
D. VAN NOSTRAND COMPANY, INC. 

250 FOURTH AVENUE 



COPYRIGHT, 1940 

BY 
ATHERTON SEIDELL 



ARGENTUM Ag 



SILVER BENZOATE 



SOLUBILITY OF SILVIR BBNZOATB IN AQUEOUS SOLUTIONS OF SALTS AT 25 

(Kolthoff and Bosch, 193?..) 



Aq. Solution 


Ota. Mola 


. per liter 


Aq. Solution Obi. Mols. 


per liter 


of: 


' Sau 


AglC fl H 5 C<!x^ 


of: r Salt 


SC&e"s 03 


KN0 3 


0.05 
0.09 
0.10 


O.01298 
0.01369 
0.01366 


Water alone o.o 
AgNO, o.oi 

11 . 02 


0.01162 
0.00786 
O.OO576 


n 


0.25 


0.01483 


" 0.03 


O.OO447 


NaNO, 
UNO* 

MgtNOglg 
Sr(N0 3 ) 2 
Ca(NO,) 2 


0.50 
0.50 
0.50 
0.50 
0.498 
0.668 
0.253 


0.01590 
0.01628 
0.01628 
0.01697 
0.01759 
0.01784 
0.01633 


" . 04 

11 0.05 

11 O.10 

Na C 6 H 6 COO o.oi 

" 0.02 

11 a.03 

" O.04 


0.00392 
O.OO328 
O.OO248 
O.OO8l6 
0.00585 
0. 004/77 
0.00396 


3 Z 


0.507 


0.01834 


" O.O5 


0.00347 


" 


1.013 


0.02079 


11 0.10 


0.00240 



SILVER Chloro, Nitro, etc. BKNZOATES. 

SOLUBILITY OP EACH SEPAPATBLY IN WATKR AT 20. 

(Ephralm and Pflater, 1925.) 

Cms. anhydrous compound 
Compound. formula. per 100 cc. sat. sol. 

Henzoate... C fl ll t ClCOOAg 0.108 

/ >, ... C 6 IU.OCH 3 .COOA- o.o r >iS 

SILVER SALICYLATI C.HU.OH.COOAg 1,2. 

One liter sat. aqueous solution contains 0.95 gm at 23. 

(Holleman, 1893. ) 

One liter sat. solution in H^O contains 0.00332 g m - mols., equal to 
0.813 gm. Ag C 6 H 4 OH.COO i, 2 at 18. (Kolthoff, 1926.) 

SILVER HEPTOATE (Onanthylate) AgC 7 Hi 3 O 2 . 



SOLUBILITY IN WATER. 

(Landau, 1893; Altschul, 1896.) 
Cms. AgC 7 H, 3 02 per 100 Cms. H 2 O. t Cms. j 



r 100 Gms. H 2 0. 



O O . 0635 (Landau) O . 0436 (Altschul) 50 . 1652 (Landau) O . 0858 (Altschul) 

10 0.0817 0.0494 60 0.1906 0.1036 

20 0.1007 0-0555 7 0.2185 0.1351 

30 0.1206 0.0617 80 0.2495 0.1688 

40 0.1420 0.0714 



SILVER CINNAMATE C 6 II 5 .CII:CHCOO Ag. 

loogms. sat. solution of silver cinnamate in water contain o.oiigms. CoH.^CH : CH 
COOAg at QiO. (Ephraim and PAstcr, 192"). 



ARGENTUM 26 

SILVER ot NAPHTHOATE Ag[C 10 H 7 COO] 
One liter H 2 dissolves 1.67 gm. Ag[C lc J} 7 COQ] at 25 - (larsson, 1927.) 

SILVER SULFONATES. 

SOLUBILITY OF EACH SEPARATELY IN WATER. (Ephraim and Pfistor, 19250.) 

Cms. anhydrous 

compound 
Compound. Formula. t". per 100 cc. sat. sol. 

Silver anthracene -i-sulfonate . ,. AgCuH 9 SO;t 20 0.059 

_2,_ 20 o . o3 i 8 

naphthalene-2- AgGjol^SOa i6.5 1.716 

-5-chlor-i-sulfonaie.. Ag.Gi H c S0 3 Cl 20 o.55i 

11 phenanthrene-2-sulfonate AgC 14 H 9 S0 3 20 -<W 

ti n n I4 n 9 3 20 0.20 

" 10 _ ' 20 0.52 

SELVES HELIANTHATE C I4 H u N 3 SO :{ Ag.2H 2 O. 

looo cc. H 2 O dissolve 0.292 gm. C 14 H 14 N 3 S0 3 Ag.2 H 2 at 20-25. 

2 y & 14 14 j j & (Slark and Delm, 1018. 1 

SILVER PALMITATE GH 3 (GH 2 ) u GOOAg. 

looocc. sat. solution of silver palmitate in water contain 0.00128 gm. C 15 H 31 COOAg 

at 20. ( Whitby, 1026. ) 

SILVEB STEARATE GH 3 (CH 2 )i c GOOAg. 

1000 cc. sat. solution of silver stearate in water contain o.ooo65 gm. C 17 H 35 COO Ag 

at 2O. ( Whitby, 1920. ) 

SILVER LAURATE, MYRISTATE, PALMITATE and STEARATE 

SOLUBILITY OF EACH, DETERMINED SEPARATELY, IN WATER AND OTHER 
SOLVENTS AT SEVERAL TEMPERATURES. 

(Jacobson and Holmes, 1916.) 

Gms. each Salt per 100 Gms. Solvent. 
Solvent. 

Water 

<c 

Abs. Ethyl Alcohol 

a a 

Methyl Alcohol 



Ether 

CN SILVER CYANIDE AgCN 

SOLUBILITY OF SILVER CYANIDE IH WATER 



I/ . 


Laurate. 


Myristate. 


Palmitate. 


Stearate. 


35 




0.007 


O.OO4 


0.004 


50 




0.007 


0.006 


O.OO4 


25 


O.OOQ 


O.OO8 


0.007 


O.OO7 


50 


O.OOQ 


0.008 


O.OO7 


0.007 


15 


0.074 


0.063 


O.o6o 


0.051 


25 


0.072 


0.067 


0.059 


0.052 


35 


0.078 


0.071 


0.062 


0.055 


50 


0.083 


0.073 


O.O66 


O.o6o 


15 


0.010 


0.009 


0.009 


0.007 



17.5 3.i7Xio" 7 0.000042 Conductivity (Abegg and Cox, 1903.) 

18.0 2,ioxio" 7 0.000028 Potent iometric (Masaki, 1930.) 

20.0 i.6nxio" 6 0.00022 Conductivity (Bottger, .1903.) 



27 ARGENTUM Ag. 

SILVER CYANIDE AgCN. 

SOLUBILITY OF SILVER CYANIDE IN AQUEOUS AMMONIA SOLUTIONS. 

(Longi, 1883.) 



at 12 
at 1 8 



100 gms. aq. ammonia of 0.998 Sp. Gr. = 5%, dissolve 0.232 gm. AgCN 
too gms. aq. ammonia of 0.96 Sp. Gr. = io% x dissolve 0.542 gm. AgCN 

One liter aq. 3 n AgNO 3 dissolves 0.0091 gm. mol. = 1.216 gm. AgCN at 25. 

(Hellwig, 1900.) 

Fusion-point data for mixtures of AgCN + NaCN are given by Truthe (1912). 



SOLUBILITY OP SILVER CYANIDE IN AQUEOUS SOLUTIONS OP 
HYDROCYANIC ACID AT 25. 

(Randall and Hal ford, 1930.) 

This system was studied by the authors as a case of equilibrium in a 
chemical reaction involving the formation of a complex ion. The satura- 
tion equilibrium is, therefore, not that of a simple solution. A small 
concentration of strong acid is produced, but the amount is so small 
that an accurate determination of the equilibrium constant is difficult. 
The assumed reaction is Ag(CN) (s)-fHCN(aq. )= H+Ag(CN) 2 ~. The measure- 
ments are expressed in terms of molalities. 

m(HCN(an.)) m(HAg(CN) 2 ) m(HCN(aq.)) ra(HAg(CN>2) 

0.0296 0.000983 0.2275 0.00424 

0.1016 0.00204 0.2325 0.00316 

0.1596 0.00245 0.3000 0.00375 

0.1780 0.00366 0.3625 0.00331 

0.1825 o. 00246 0.4230 0.00400 

0.2124 0.00292 0.4260 0.00511 

0.2245 0.00272 0.4465 0.00427 



Similar determinations of the solubility of Silver Thiocyanate in 
aqueous solutions of Potassium Thiocyanate at 25 and the assumed re- 
action which occurs, is as follows. 

AgCNS Is. 1 + CNS" = Ag(CNS) 2 * 

Original m (KCNS) (AgCNS) m (KCNS (fre)) 

0.312 0.00202 0.310 

0.564 0.0121 0.512 

0.870 0.0458 0.824 

1.124 O.Q985 1.026 

These results cannot be accounted for by the formation of the single 
complex ion Ag(CNS) 2 " 



> iN&T- 



\ 



ARGENTUM 28 

SOLUBILITY OF SILVER CYANIDB IM AQUBOUS SOLUTIONS 
OF POTASSIUM CYANIDE AT 25 AND Vic* VBRSA. 

(Basse CD and Corbet. 1924.) 
jf* 
/ Gms. per 100 #m.<. saf. sol. Cms per 100 gms sht. sol. 

KCN. Ag ON. Phase. KCN. AgCN. Phase. 

41.7 o.oo KCN 20.14 ai.66 KAg(CN)i 

40.77 6.52 8.56 i6.ii 

39.91 8.14 8.o5 15.76 KAg 2 (CN) :J .lLO 

40.24 10.98 8.93 17.73 

40.44 13.71 KAg(CN) 4 .H,O 6.75 i3.53 AgCN 

37.76 18.92 2.36 4.42 

35.19 ^5. i 8 r.64 3.27 

28.43 26.37 KAg(CN)' i.a6 2.3i 

26.67 24.71 2.16 trace ) 

ftote. Due to the difficulty of obtaining KCN free of KOH the sat- 
urated solutions were prepared from double salts which could be obtained 
free of KOH. Saturation was reached by constant rotation in wax bottles, 
in which an atmosphere of coal gas, washed by passing through solutions 
of lead acetate and sodium hydroxide, was maintained. Both* the liquid 
and solid phases were analyzed. 

100 gms. liquid S0 2 dissolve 0.019 gm. AgCN at o. (Jander and 
Ruppolt, 1937.) 

CN 

SILVER DICYANIMIDE AgN(CN) 2 

One liter saturated solution in water contains 0.0064 gm. AgN(CN) 2 at 
i8-20, determined by the potentiometric method. (Birchenbach and 
Huttner, 1930.) 



SILVER TRICYAH METHYL AgN(CN) 3 

One liter saturate solution in water contains 0.013 gm. -AgN(CN) 3 at 
i8-20, determined by the potentiometric method. (Birckenbach and 
Huttner, 1930.) 



SILVER FERRICYANIDE Ag 3 FeCN 6 . 

One liter H 2 O dissolves 0.00066 gm. Ag 3 FeCN 6 at 20. 

(Whitby, iyio.) 

SILVER SODIUM CYANIDE AgCN.NaCN. 

100 gms. H 2 O 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. HO dissolve 4.7 gms. at o, and 7.4 gms. at 16. (Fronmiillcr, 1878.) 



PREFACE 

The first edition of this compilation, comprising 353 pages, appeared in 
1907. A completely revised second edition, containing 756 pages of tables, 
was published in 1919- Due to the high cost of printing tables," .the new 
material collected after 1919 could not be economically combined with that 
already published, and was issued in 1928 as a supplementary volume of 500 
pages. This plan cannot be repeated, since the searching of desired data in 
a series of three volumes would be awkward. Therefore a complete revision 
of the compilation has become necessary. 

The cost of printing by the usual method has not declined and the amount 
of new data to be added has continued to increase. Consequently, the publi- 
cation of a completely revised edition would not have been possible except 
by taking advantage of the economical process of off-set printing, and the 
new developments in the microfilm copying of printed pages. The present 
compilation is accordingly, an example of the type of compendia of experi- 
mental research which these two applicationsof photography have made possible. 

Due to the very large amount of quantitative solubility data which is 
now available, its publication in a single volume of convenient size is no 
longer possible. Therefore, it has been decided to include all data upon in- 
organic and metal organic compounds in one volume, and the results upon the 
compounds of carbon in a second volume. 

Advantage has also been taken of this circumstance to change the manner 
of arranging the data. The alphabetical plan based on the English names of 
the compounds has been changed to one having the symbols of the elements as 
the basis for the alphabetical arrangement. This purely chemical system of 
presenting the data will be more convenient to chemists having an imperfect 
knowledge of English, and in addition, makes it possible to use the symbols 
as guiding marks for locating desired results. For this purpose the symbols 
of the basic constituents of the inorganic compounds are placed at the upper 
outer corner of the pages, and those identifying the acidic constituent, and 
thus the particular compound in each case, are placed lower down on the outer 
margins of the pages. 

In accordance with the principle adopted for previous editions, the re- 
sults for systems of two or more compounds are always entered under that one 
of which the initial letter of its formula comes first in the alphabet. This 
has the effect of causing the larger amount of the data to be placed under 
the first letters of the alphabet. With this single rule in mind it should 
always be possible to find results for particular systems, but not always 
for each separate compound of which they are composed. In order to provide 
for those cases in which results are given in other than the expected alpha- 
betical position, a formula index, serving the purpose of cross references, 
is given at the end of this volume. 



The procedure by which the new material has been collected differs from 
that previously followed in that, thanks to microfilm copying, it has no 
longer been necessary to manually transcribe from each original paper the 
data to be subsequently used. It has simply been necessary to note the 
Capers found by perusing the periodicals, and have these photographically 
copied on microfilm. These microfilm copies then become the source material 
from which the compilation is made. This not only effects a saving in the 
effort required to collect the original data but reduces by one-half the 
errors due to copying. 

When microfilm copies of all papers published since 1927 had been col- 
lected, the formulae of the compounds for which results were given in each 
case", were written on a sheet of paper to which the microfilm copy was at- 
tached. With the aid of these notations the new results could be alphabeti- 
cally assembled with those taken from the preceeding volumes. Thus all 
available results upon each compound or system were brought together for 
comparison and selection of the final values to be included in the new book. 
The actual compilation could then be made without further recourse to the 
periodical collections in libraries, and under conditions particularly favor- 
able for the orderly arrangement and accurate presentation of the data. 

In reference to the manner in which the pages of the new book have been 
prepared for planographic reproduction, it is necessary to call attention to 
certain imperfections which have resulted. Since these pages are composed 
of tables reproduced from the volume printed in 1918, in the United States, 
and the supplementary volume printed in 1927, in France, together with the 
tables of new data typewritten on a"Varityper" and photographically reduced, 
a considerable variet^ of type size and design has resulted. This Variation 
in typography is to be regretted but the expense of completely resetting the 
book would have prevented its publication. 

In addition to the typographical variations, a perceptible reduction in 
sharpness of definition of the print will be noted in some cases. This re- 
sults from the two fold photographic reproduction of the new tables, and the 
slight imperfection of some of the old pages. It is hoped that these defi- 
ciencies in uniformity, and occasional indistinctness of the typography will 
not diminish the value of the compilation to those having need of it in their 
work. This plan of combining the previously collected data with the new, 
has made it possible to prepare a more nearly complete collection of solu- 
bility data, at a far less expense, than would have been possible by the 
usual methods of printed publication. 

Another point about which a word of explanation should be given is the 
variation in nomenclature resulting from the use of the latin names, such 
as argentum, aurum, kaliizm, natrium, plumbum, etc., from which the symbols 
used in the alphabetical arrangement, were derived. In these cases, the 
cost of changing the English names in the titles of the tables reused from 



the previous edition, did not appear warranted. Furthermore, it is recog- 
nized that in spite of the advantage of the adoption of the Latin names, in 
rendering the language of chemistry more universal, there are many persons 
who prefer correctness of expression in their own language, to the more gen- 
eral and precise comprehension of the chemical information imparted. Although 
the English names are retained in the majority of cases, it is hoped that 
eventually an international system of naming chemical compounds will be de- 
veloped. This would make the names of the substances with which chemists are 
concerned, as universal as the chemical symbols of which they are composed. 

The general practice observed in previous editions of this compilation, 
with respect to limitations of scope and orderly presentations of the numeri- 
cal results has been followed in the present one.' Since the name alone does 
not always accurately identify a compound, greater precision has been sought 
by giving the chemical formula as well. In a few cases, however, due to lack 
of information in the original papers this could not be done. It should be 
mentioned also that occasionally the original results are presented in terms 
which are not accurately defined. Considering the effort involved in the 
quantitative determination of solubilities, it is regret able that authors some- 
times fail to mention details essential to the precise comprehension of their 
work. 

The brief remarks in connection with some of the tables are intended to 
indicate the general character of the experiments, the methods ,used, and the 
probable accuracy of the results. The absence of such remarks may be taken 
to mean that the determinations presented no exceptional diff iculties > that 
they were made by the usual methods, and with acceptable care. For those 
cases where incomplete results are given or more information than is quoted 
in the present compilation is desired, a microfilm copy of the original paper 
may be obtained, at very little expense, by sending the exact reference to 
Bibliofilm Service, in care of the Library, U. S. Department of Agriculture 
Washington. D. C. 

In conclusion, I wish to thank those who have called my attention to 
errors in the previous editions, and mention that I will be equally grateful 
to those who take the trouble to notify me of mistakes in the present volume. 

I am greatly indebted to Mr. Leslie J. Robinson for the painstaking 
manner in which he has made the Varitype copies of all new tables, and to 
Mr. John R. Van Cott for combining these with the tables reused from the 
previous volumes in the final form here shown. 

A. S. 
Washington, D. C., March 30, 1940. 



ABBREVIATIONS 



Most of the following abbreviations will be found written both with capitals 
and without. 



[a]x>. Specific Rotation. 

abs. Absolute. 

abs. coef. Absorption Coefficient. 

alcohol. Ethyl Alcohol. 

amt(s). Amount (s). 

anhy. Anhydrous. 

aq. Aqueous. 

atrn(s). Atmosphere(s). 

at. wt. Atomic Weight. 

b.-pt. Boiling-point. 

C. Centigrade. 

calc. Calculate(ed). 

cc. Cubic Centimeter(s). 

cm. Centimeter(s). 

coef. Coefficient. 

com. Commercial. 

compd. Compound. 

cone. Concentration, Concentrated. 

cond. Conductivity. 

const. Constant. 

cor. Corrected. 

crit. Critical. 

cryo. Cryohydric. 

cryst. Crystalline. 

d. Dextro (in connection with the 
name of an optically active com- 
pound). 

^. Density (d w Specific Gravity 
at 1 8, referred to water at 4; d^ 
at 20 referred to water at 20). 
decomp. Decomposition, 
dif. Different, 
dil. Dilute. 

dist. coef. Distribrrion Coefficient. 
ed. Edition, 
elec. Electric(al). 
equil. Equilibrium. 
equiv. Equivalent (s). 
eutec. Eutectic. 

F. F ahrenheit. 

f .-pt. Freezing-point. 
g- gm- gms. Gram(s). 
gm. mol. Gram Molecule(s). 

G. M. -Gram Molecule(s). 
hr(s). Hour(s). 

*. (<* + Inactive (in connection 
with the name of an optically active 
compound.) 



inorg. Inorganic. 
insol. Insoluble. 

/. Laevo (in connection with the 
name of an optically active com- 



kg. kgm. Kilogram (s). 
1. Liter (s). 
mm. Millimeter (s) 
m. Meta. 
max. Maximum. 
mg., mgm. Milligram (s). 
mol(s). Molecule(s), Molecular. 
mol. wt. Molecular Weight. 
millimol. Milligram Molecule. 
m.-pt. Melting-point. 
. Normal (gm. equiv. per L). 
N. Normal (used rarely). 
o. Ortho. 
ord. Ordinary. 
org. Organic. 
p. Page. 
p Para. 
pet. Petroleum. 
ppt. Precipitate. 
pt. Point. 

quad. pt. Quadruple Point. 
qual. Qualitative. 
sapon. Saponification. 
sat. Saturated. 
sol(s). Solution(s). 
sp. gr. Specific Gravity (Density). 
sq. cm. Square Centimeter. 
5. Symmetrical. 
sym. Symmetrical. 
t. Temperature, Centigrade Scale. 
temp(s). Temperature (s). 
tr. pt. Transition Point. 
vol(s). Volume (s). 
undissoc. Undissociated. 
U. S. P. U. S. Pharmacopoeia. 

wt. Weight. 

oo Infinity. 

.10""*, .io~~ 5 , etc., following a result 
means that the decimal point is to be 
moved as many places to the left as 
indicated by the minus exponent. 



ARGON 



ARGON 



SOLUBILITY OF ARGON IN WATER 

(Lannung. 19TO; Von Antropoff, 1919.) 
Lannung 





5 

10 

15 

20 
25 
30 
35 
40 
45 
50 



a 


1 


0.0560 





0.0460 





0.0405 


0.0425 


0.0365 


O.O391 


0.0336 


0.036l 


0.0310 


0.0342 


0.0288 


0.0321 


0.0270 


0.0305 


0.0252 


0.0290 


O.O237 


0.0278 


0.0223 






Von Araropoff 
B 

0.0580 
0.0500 
0.0450 
0.0408 
0.0374 
0.0350 
0.0327 
0.0305 
0.0286 
0.0270 
0,0257 



a "" Bunsen Absorption Coefficient which shows the volume of gas (at o 
and 760 mm. fig. pressure) dissolved by one volume of solvent at the 
given temperature when the partial pressure of the gas is 760 mm. Hg. 

i *= Ostwald Partition Coefficient which is the equilibrium distribution 
ratio of the volume concentrations of the gas in the solution and in the 
vapor phase. The relation between i and a is, i~ aT/273 where T is the 
absolute temperature at which the measurement was made. 

B Kuenen's modification of the Hunsen Absorption Coefficient in which 
one gram of solvent is substituted for one cubic centimeter of solvent. 

The results in the above table were read from curves plotted from the 
data given by Lannunfj; and von Antropoff. In both cases the determina- 
tions were- made with great care, lannunf; points out that the previous 
measurements of Bstreicher, 1899 are uncertain on account of the small 
volume of gas, the large amount of dead space in his apparatus and the 
difficulty of measuring the volume of gas in the dry state. 

SOLUBILITY OF ARGON IN SEVERAL SOLVENTS 



15 
18 

20 

25 

30 
37 



Methyl Alcohol 

__?!__ 

a i 

0.253 0.267 
0.251 0.267 
0.250 0.268 



(Lannung 19ITO.) 
Ethyl Alcohol 



Acetone 
(CH,) .CO 



0.243 
0-240 



0.270 



0.243 


0.256 


0.271 


0.286 


0.242 


0.258 


0.271 


0.290 


0.24.0 


0.258 


0.273 


0.293 


0.237 


0.258 


0.274 


0.299 


0.234 


0.260 


0.276 


0.306 


0.231 


0.262 


0.279 


0.317 



Cyclohexane 



Cyclohexanol 
(CHJ K CHOH 



15 





.220 





.232 





.308 





.325 


18 





.221 





.236 





.307 





.327 


20 





.221 





.237 





.306 





.328 


25 





.222 





.242 





.305 





-333 


30 





.222 





.246 





.304 





337 


37 





.222 





.252 





.303 





-344 



0.112 0.112 
0.113 0.125 
0.114 0.129 



ARGON 



SOLUBILITY OF ARGON IK WATER AND IN 
SEVERAL SOLVENTS AT HIGH PRESSURES 

(Sissklnd and Kasarnowsfci, 1931, 1933.) 

A steel bomb of about 100 cc. capacity, as described by Ipatiew, Jr., 
Drusking-Artemowitsch and Tichomirow, 1932, vras used. 



Solvent 



Pressure cc.A per 1 cc. 

In Solvent at 

Atmospheres Pressure P 

P VT. 



Corrected 



Calc. 
Bunsen 
Absorp. 

Coef. 



H ? 



+0.2 



0.0515 0.0515 

1.29 0.05i6 

2.52 0.0504 

3.50 0.0467 

4-35 0.0435 

5.06 0.0405 

0.262 0.262 

7.76 0.310 

16.2 0.325 

23.8 0.317 

30.9 0.309 
0.251 0.251 
7-57 0.303 

15.8 0.315 

22.8 0.304 

27.5 0.275 

0.554 

0.238 

1.32 

0.106 

Data for the solubility of Argon in distilled water and in sea water, to- 
gether with a critical discussion of the literature, are given by Coste, 
1917. 

One liter of cyclohexanol dissolves 171 .21 cc. Argon at 26 and 755 mm Hg. 
pressure (Cauquil, 1927.). 

SOLUBILITY OP ARGON IN AQUEOUS SALT SOLUTIONS AT 25 

(Xkerlbf, 1935.) 



C 2 H 5 OH 



(C 2 H I 

<cH,rco 

CH (CflJ.CH, 



1 


0.0515 


25 


1.25 


50 


2.46 


75 


3.43 


100 


4.27 


125 


4-95 


1 


0.262 


25 


7.56 


50 


15.8 


75 


23.2 


100 


30.1 


1 


0.251 


25 


7-39 


50 


15.4 


75 


22.3 


100 


26.9 


25 


13.8 


25 


9.31 


25 


33.0 


25 


2.67 



Sal 


Mols Salt per 






1000 gns. H ? 


a 


None 


=H 


0.0332 


KC1 


3.00 


0.0220 


" 


4.55 


0.0174 


NaCl 


3-23 


0.0216 


n 


5.98 


0.0149 


LiCl 


3.35 


0.0248 


" 


6.78 


0.0l87 


NaN0 3 


3.51 


0.0204 




7.37 


0.0123 


acio 4 


4.05 


0.04H 




9.32 


0.0521 





hois Salt per 




C 


1000 gms. H 2 


a 


CaCl 2 


2.95 


0.0216 


" 


5.37 


O.OlSo 


SrCl 2 


2.10 


0.0203 


" 


3.56 


0.150 


BaCl 2 


1.25 


0.0l85 


11 


1 .74 


0.0141 


MgClg 


3.02 


0.0248 


" 


5.02 


0.0228 


A1C1 3 


0.98 


0.0247 


II 


0.56 


0.0179 



Data for the solubility and- diffusion of argon in solid and liquid 
metals are given by Sieverts and Bergner, 1912. 
Palladium, activated by thermic treatment in a vacuum absorbs 319 
volumes of argon, Klarmann, 1930 



ARGON 



SOLUBILITY OP ARGON IN SEVERAL SOLVENTS 
AT HIGH PRESSURES 

(Sissklnd and KasarnowsKl, 1931, 1933.) 



Solvent t 


Pressure 
In 


Atmospheres 


Acetone o 


50 


" o 


100 


n Propyl 




Alcohol o 


50 


n Butyl Alcohol o 


50 


I so Butyl 




Alcohol o 


50 


Sec. Butyl 




Alcohol o 


50 


Iso Amy) 




Alcohol o 


25 


Iso Amyl 




Alcohol o 


50 


n Hexyl Alcohol o 


25 


n Octyl Alcohol o 


50 


Sec. Octyl 




Alcohol o 


25 


Benzyl Alcohol o 


25 


Benzyl Alcohol o 


50 


Cyclohexanol 25 


50 


Methyl Ethyl 




Ketone o 


25 


Methyl Propyl 




Ketone o 


50 



Calc. 
Bun sen 
Absorp. 

Coef. 



0.249 
0.254 

0.220 
0.209 

0.228 



0.210 

0.210 

0.174 

(0.190) 

O.l63 

0.172 
0.060 
0.060 
0.112 

0.222 
(0.239) 

0.234 



Solvent 



Diet.hyl Ketone o 
Methyl Hexyl 

Ketone o 
Ethyl Prot>yl 

Ketone 
Cyclohexanon 



0.210 Benzene 



Toluene 



Xylene 



Cyclohexane 
Methyl 

Cyclohexane 25 
Benzyl Ether o 



Pressure 


Caic. 
Bunsen 


In 
Atmospheres 


Absorp. 
Coef. 
a. 


50 


0.237 


50 


0.193 


50 


0.238 


50 


0.127 


100 


0.128 


50 


0.124 


50 


0.197 


100 


0.203 


125 


0.204 


25 


0.200 


50 


0.200 


75 


0.214 


50 


0.195 


50 


0.196 




(0.205) 


100 


0.211 


50 


0.302 


50 


0.311 


25 


0.068 


50 


0.069 


100 


0.072 



ACTINIUM EMANATIONS. 

SOLUBILITY IN SEVERAL SOLVENTS. 

(Hevcsy, 1912.) 

A method was elaborated for determining the partition coefficient between a 
gas and a liquid phase. The solubility of actinium emanations was then de- 
termined in KC1, H 2 O, H 2 SO 4 , C 2 H 6 OH, C 6 HuOH, (CH 3 ) 2 CO, GH ft CHO f CJI, 
C?Hs, petroleum ether and CS 2 . The solubility increases in the order named. 
Close relations are indicated between actinium, thorium and radium. 



Experiments are described by tmre, 1927, upon the separation of KaAc 
by means of distribution studies. Since iron can be removed from its 
hydrochloric acid solution by extraction with ether, this principle was 
applied to the separation of RaAc. Nitric acid was substituted for 
hydrochloric acid. Results are given for the extraction of aqueous 
nitric acid solutions of thorium by means of ether, and similar results 
for nitric acid actinium solutions. This method failed to separate- 
RaAc into two components, thus furnishing new evidence of its unity. 



ARGENTUM 
ARGENTUM 

SILVER, Ag: 



SOLUBILITY OF SILVER IN WATER 
(Krepelfca and Toul, 19250 



Silver of purity sufficient for atomic weight work was employed. 
Thin leaves of it were placed in contact with highly purified and 
freshly distilled water in completely filled and tightly stoppered 
Krlenmeyer flasks, on the one hand and in silver flasks on the 
other. The flasks thus prepared were kept in the dark at i8-20C. 
and shaken from time to time. 

For analysis the water from the vessels was poured into a quartz 
dish and carefully evaporated in the dark to 60-80 cc. The Ag in 
this solution was determined by nephelometric comparisons with known 
standards. Maximum solubility was reached in 21 days and corres- 
ponded to 

0.035 m R- Ag. per 1000 cc. water. 

Silver sheets, the surface of which had been previously reduced 
by pure dry hydrogen at 400 showed no solubility as measured by 
nephelometric tests. Hence it follows that the dissolution of 
silver is caused by its surface oxide, or by oxygen on its surface 
or dissolved in the water. Measurements made in glass vessels 
were, on the average 0.003 mg. higher than those made in silver 
vessels. This difference is probably due to the influence of 
alkalies dissolved from the glass. 

Determinations of the solubility of silver in distilled water 
are also given by Freudlich and Sollner, 1928. Using 40 sq. cm. 
of silver surface per 100 cc. of water and a contact period of 3 
days, 0.025 rag- Ag per liter were found. The analyses were made 
by Ilaber et al, 1926, microclokimastic method. 

TITB SOLUBILITY OF SILVER IN MERCURY 

(Sunler and Hess, 1928: De Right, 1933.) 

Highly purified Hg and excess of pure Ag were agitated together 
by gentle rocking in an evacuated tube provided with a side bulb 
into which the saturated solution could be filtered through glass 
wool by inverting and allowing air to enter the apparatus. 
Equilibrium was approached from both sides at each temperature. 
The analyses were made by distilling the mercury from the filtered 
saturated solution at 200 under vacuum or by volatilizing it in 
a stream of Hydrogen at 270-300, and weighing the residual 
silver. The results are expressed in terms of gram atoms of Ag 
per 100 gram atoms of Ag Hg. The authors discuss previous 
published determinations. 

r o Atomic ,o Atonic r o Atonic 

c Percent Ag c Percent Ag L Percent Ag 

1O O.O*8 60 0.190 120 0.587 

2O O.O66 70 0.2^1 140 0.797 

30 0.088 80 0.288 l6o 1.053 

14.0 0.114 90 0.352 l8o 1.356 

SO O.14.7 1OO 0.419 200 1.708 



5 ARGENTUM 

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. 

Results for the solubility of Ag in Cu, determined by hardness 
measurements are given by Hansen, 1930; and determinations by the 
X ray method are given by Agnew and Sacks, 1930. 

Data for the distribution of silver between Zn -f Pb, Zn -f Bi, Al -f Pb, Al -f Bi r 
Zn + Tl and Al + Tl are given by Tammann and Schaftmeisler, 1924 - 

Data for the equilibrium between melted silver and the chlorides 
of Cu and Pb are given by Tubandt and Munzing, 1927. 

SILVER ARSENATE Ag 3 AsO 4 . 

One liter H 2 O dissolves 0.0085 g m - Ag3AsO4 at 20. (Whitby, 1910.) 

SILVER ARSENITE Ag 3 As0 3 . 

One liter HaO dissolves o.oi 1 5 gm. AgaAsOaat 20. (Whitby, 1910.) 

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 dextrine, starch, sugar etc., is 
proportional to the amount of silver present. 

SILVER BORATE AgB0 2 . 

One liter of aqueous solution contains about 9.05 gms. AgBOo at 25. 

(Abegg and Cox, 1903.) 
SILVER Dl BORATE Ag 2 C.2B 2 3 .2H 2 

The System Ag 2 + B 2 3 + H g O at 19 

(toilet, 1930) 

Ctoia. per 100 ens. Solid OAS. per 100 gms. Solid 

Sat. Solution Phase Sat. Solution Phase 



0.16 o.i Ag 2 0.2B 2 3 , 2 H 2 0.91 3-51 Ag 2 0. 2 B 2 3 .2H 2 (>fBlOIl), 

0.22 0.75 " -70 3-3 ' B(OH) 3 

0.33 1.4 " 0.35 2.9 "' 

O.55 2.2 " 0.0 2.6 



SILVER Tri Antipyrine BORO FLUORIDE Ag(COC 10 H 12 N 2 )- 5 BF 4 

100 cc sat. solution in H 2 contain 17.7 gms. salt at 20. 

(WiUce-Dorfurt and Murecit, 1929) 

SILVER BROMIDE AgBr. 

SOLUBILITY IN WATER. 

t Gtaa. AgBr per Liter. Authority 

i8(?) 0.00029 (Hahn and Schulze, 1927.) 

18 0.00012 (Kolthoff, 1921.) 

18 0.000131 (Masaki, 1930.) 

20 0.000084 (Bbttger Z. physik. Ch. 46, 602/03.) 

25 0.000137 (Abegg and Cox 2. physik. CU. n6, 11, '03.) 

100 0.00370 (Bottger Z. physik. Ch. s6,93 '06. ) 
(See also Holleman Z. physik. Ch. 12, 129, '93; Kohlrausch Ibid, 50, 365* "05.) 



&.g ARGEHTUM 



SOLUBILITY OP SILVER BROMIDE IN WATER AND IN AQUKOUS SOLUTIONS 
op ACIDS AND SALTS. 

(Bedell. 1938.) 

The method (see Bedell, 1937} consisted in alternately adding, drop- 
tfise, o.ooi normal solutions of silver hydroxide and hydrobromic acid 
to looocc of water at the chosen temperatures. The point at which a 
precipitate appeared was determined by observing the diffraction of a 
beam of light passing through the solution. 

GW. AgBr per 

liter sat. sol. 

20 0.00035 

40 . O.00066 

60 0.00112 
80 



Using the above method, but substituting o.ooi normal silver nitrate 
or silver sulfate for the hydroxide and various bromides for the hydro- 
bromic acid, the author obtained results, at about 20, for the solu- 
bility of silver bromide in aqueous solutions of KNCL, LiNO , Ba(NCL> ? , 
MntKOgJg, HN0 3 , H ? S0 4 , Hg(N0 3 ) ? and IlgS0 4 , varying in concentration ' 
between 0.0004 ^^ 0.0252 gms. per liter. The results showed that with 
the exception of mercuric nitrate and sulfate only a very slight increase 
in solubility of the AgBr occurred. The increase in solubility with the 
mercury salts confirms the previously reported exi stance of compound 
formation, between silver bromide & mercury salts. 

SOLUBILITY OF SILVER BROMIDE IN AQUEOUS AMMONIA SOLUTIONS. 

(Longi Gazz. chim. ital. 13, 87, '83; at 80, Pohl Sitzber. Akad. Wiss. Wien, 41, 267, '60.) 

Cms. AgBr at 12 per Cms. AgBr at 80 pet 

Solvent. I000 cc . I000 Gms> 1000 Cms. 

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. o .986 ... ... o . 51* i .of 

* Dried AgBr. t Freshly pptd. 

SOLUBILITY IN AQUEOUS SOLUTIONS OF AMMONIUM BROMIDE AND OF GELATIN. 

( Winthcr, 1023, 1924. ) 

The determinations were made by measurements of the electromotive force of a 
series of elements of the type. 

Ag 1 o. i rc AgN0 3 | Aq. io/o NH 4 NO,| x \ Ag, 

where a: is a mixture of Ag Br and of the solution in which its solubility is to be 
measured. Two identical elements were measured for each solution. The potential, 
TC, very soon attained a constant value which did not change for many Lours. 
The mean value for the exponents of the solubility products in solutions composed 
of various mixtures of ammonium salts, gelatin and erythrpsine, was 11.92. Since 
the solubility product in all of the solutions had the same value it was concluded 
that the solubility of silver bromide in water is not altered by the addition of 
gelatin, erythrosine and small amounts of NH 4 T and NH 4 Cl. By the addition 
of bromide the solubility is decreased in accordance with the law of mass action. 
Fusion-point data for mixtures of Ag Br + Na Br are given by Zcmcznzny, 1926. 



SILVER BROMIDE 



ARGENTUM 



SOLU 

Res 

(Bo< 

<*16.5 Of 

Sat. Sol. 
0.9932 

0.9853 
0-9793 
0.9720 

0-9655 


UIUTY OF SILVER BROMIDE IN AQUEOUS AMMONIA SOLUTIONS. 
suits at 15. Results at 25. Results at 25. 

dlander, 1892.) ( Bodlander and Fittig, 1901-02.) ( Whitney and Mclcher, 1903.) 
Cms. Mols. per Liter. Gms. Mols. per 1000 Cms. H 2 O. Concentration per Liter. 


NH 3 . 
1.085 

2.365 
3.410 

4.590 
5.725 


Ag 2 Br 2 . 
O.OOII 

0.0031 

0.0050 
0.0074 

O.OIOI 


o 
o 
o 
I 

3 
5 


NH 3 . 
.1932 

.3849 

-7573 
965 
.024 
.244 


o 
o 
o 
o 
o, 
o, 


AgBr. 
.OOO6O 
.00120 
.OO223 
.00692 
.01163 
.02443 


G. Mols. NH 3 . 
0.0764 
O.II5 
0.268 
0.273 
0.450 
0.497 


G. Atoms Ag. 
O.OOO276 
O.OOO39I 
O.OOO94I 
O.OOI07 
O.OOiyO 
O.OOI59 



SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF: 



Ammonia at o. 
(Jarry, 1899.) 

Grams per 100 cc. Solution. 



Monomethyl Amine at 11.5 
(Jarry.) 

Gms. per 100 cc. Solution. 



NHa Gas. 


AgBr. 


NH 3 Gas. 


AgBr. 


3-07 


O.o8o 


26-27 


I .067 


4.88 


0-096 


31.26 


1.568 


6.69 


0.172 


33-89 


1.987 


8.29 


O-2I2 


3 6 -52 


2 .669 


11.51 


c-349 


37.22 


2.888 


I5-32 


o-557 


37-70 


2.930 


18.09 


0.722 


39.26 


2 .892 


19-53 


0-741 


39-95 


2.852 



NH 2 CH 3 . 


AgBr. 


II .01 


O.07 


13 -17 


O.I2 


15 .13 


0.16 


17.97 
32.58 

35 - 62 


0.28 

o-55 
o-73 


43-n 
48.44 


i .27 
2.89 



SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF METHYL 
AMINE AND OF ETHYL AMINE AT 25. 

(Bodlander and Eberlein, 1903; Wuth, 1902.) 
In Methyl Amine. In Ethyl Amine. 

Mols. per Liter. Mols. per Liter. 

Total Base. AgBr. Free Base.* Total Base. AgBr. Free Base.* 

1.017 0.0025 i.oi2(B.&E.) 0.483 0.00231 o.478(B.&E.) 

0.508 0.0013 o.5o5(B.&E.) 0.200 0.00097 0.198 " 

0.203 0.00049 0.202 (B.&E., W.) o. 100 0.0004750.099 
o. 102 



0.103 0.000711 
0.06572 0.000258 
0.05512 0.000193 
0.03942 0.000137 
0.01272 0.0000867 



(W.) 



0.00026 0.102 (B.&E.) 

0.0947 0.00041 ... (W.) 

0.051 0.00012 0.051 (B.&E.) 

o . 04 o . 00034 . . . (W.) 

0.02 0.00026 ... (W.) 

* The free base is found by subtracting from the total base two mols. of base for each atom of dissolved Ag. 

SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF MERCURIC 
NITRATE AT 25. 

(Morse, 1902.) 

Mols. HgNOr Mols. AgBr Gms. AgBr 
(HNOa) per Liter. per Liter. per Liter. 

I 0.03660 6.878 

o.io 0.00873 1.640 

O.O5 0.0063.9 I.2OO 

Since HN0 3 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 HNOs. Both crystallized and 
amorphous silver bromide gave identical results. 



Mols. HgNO r 


Mols. AgBr 


Gms. AgBr 


(HN0 3 ) per Liter. 


per Liter. 


per Liter. 


0.025 


0.00459 


0.863 


O.OI25 


o . 003 29 


0.618 


O.OIOO 


o . 00306 


0-575 



A ARGEHTUM 8 

SILVER BROMIDE 

SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SALT SOLUTIONS. 

(Mees and Piper, 1912.) 



Aqueous Solution. t. 

Aq. i per cent Sodium Thiosulf ate ? 2 . 06 

" " Ammonium Thiocyanate " 0.03 

" " Ammonium Carbonate " 0.004 

" Sodium Sulfate " 0.055 

" Thiocarbamide " 1.49 

SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SALT SOLUTIONS. 

(Valenta, 1894; see also Cohn, 1895.) 

Gms. AgBr per 100 Cms. Aq. Solution of Concentration: 

Salt Solution. t. , --- * -- > 

1:100. 5:100. 10: 100. 15:100. 20:100. 

Sodium Thio Sulphate 20 0.35 1.90 3-50 4.20 5.80 

" " Calc. by Cohn. 20 0.50 2.40 4.59 6.58 8.40 

Sodium Sulphite 25 ...... o .04 ... o .08 

Potassium Cyanide 25 ... 6 .55 ......... 

11 Calc. by Cohn 25 ... 6.85 ......... 

Potassium Sulphocyanide 25 ...... o - 73 ...... 

Ammonium Sulphocyanide 20 ... 0.21 2.04 5.30 

Calcium Sulphocyanide 25 ... ... o . 53 

Barium Sulphocyanide 25 ...... 0.35 ...... 

Aluminum Sulphocyanide 25 ...... 4 . 50 ...... 

-a Thio Carbamide 25 ...... 1.87 ...... 

r Thio Cyanime 25 0.08 0.35 0.72 

NOTE. Cohn shows that the lower results obtained by Valenta are due to the 
excess of solid AgBr used and the consequent formation of the less soluble di salt, 
3(AgS20 3 Na)j, instead of the more soluble tri salt, (AgSaOaNa^^SjOa. 

loo cc, HjO containing 10 per cent of normal mercuric acetate, Hg(C 2 H 3 O2)2-f 
Aq., dissolve 0.0122 gm. AgBr at 20. 

100 grns. 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 m - AgBr 
at 15. (Schierholz, 1890^ 

SOLUBILITY OF SILVER BROMIDE IN AQUEOUS POTASSIUM BROMIDE AT 25. 

(Hellwig, 1900.) 

Mols. KBr per Liter 2.76 3.68 4.18 4.44 4.864 
Gms. KBr per Liter 2.20 7.50 13-50 17. 95 26.44 

SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF SopiuM SULFITE, 
Results at Room Temperature (?). Results at 25. 

(Mees and Piper, 1912.) (Luther and Itcubncr, 19 m.) 



Gms. 


JXT Liter. 


Gms. per Liter. 


Gms. Formula Weights 
per Liter. 


NasSQi. 


ARBr. 


NajSO,. 


A K Br. 


SO,". 


Ag'. 


0.08 


0.000746 


4.85 


0.0329 


0.232 


O.OO25 


0.17 


O.OO2I9 


9-47 


0.05264 


0.406 


O.OO23* 


0.30 


0.00393 


I7-65 


0.116 


0.448 


O.O023* 


0-59 


O . OO44cS 


3^.2 


0.265 


. 466 


0.0053 


l -*3 


0.00865 


70.75 


o-57 


0.474 


0.0055 


2.08 


0.01585 


83.75 


0.79 


0.675 


O.OO84 



SILVER BROMIDE 



SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF SODIUM 
THIOSULFATE AT 35. 

(Richards and Fabcr, 1899.) 



Cms. Cryst. Na % 

Thiosulfatc 

per Liter. 

IOO 
200 
300 
400 



Cms. AgBr 
Dissolved per Gm. 
of Thiosulphate. 

0.376 
0.390 

o-397 
0.427 



Mols. AgBr 

Dissolved per 

Mol. of 



0.496 

0-SI5 
0.524 
0.564 



loo cc. of 3 n AgNO 3 solution dissolve 0.04 gm. AgBr at 25. (Hcllwig, 1900.) 



SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OP 
POTASSIUM THIOCYANATR AT 25. 

(Randall and Hal ford, 1930) 

This system was studied by the authors as a case of equilibrium in 
a" chemical reaction involving formation of a complex ion. The assumed 
reaction is Ag Br s--2 CNS~ * Ag (CNS)g"~+Br~, but the sulubility cannot 
be accounted for by the formation of a single complex ion Ag(CNS)~. 
The results of the analyses of the saturated solutions are expressed 
in molalities. 



Bi 



Total (KSCN) 



2510 

2702 

5205 

5819 

7577 

0.7762 

1 .0089 



(Ag Br) 

0.0011 
0.0012 

0.0095 
0.0085 
0.0285 
0.0307 
0.0663 



free (KCNS) 

0.249 
0.267 
0.501 
0.564 
0.701 
0.715 
0.875 



SOLUBILITY OF SILVER BROMIDE IN CONCENTRATED SOLUTIONS 
OF HALOGEN SALTS. 

(Dede and Wanner, 1927.) 



Molecular Wt in Oma nf * Mllllmols AgBr dlaeolved In one On. 

nOJ.BCU.Ltir Wfc. in UBS. Of P/ilt t\t QnlvAnr at- 

^ompoaltlon of 1 Om Equlv of Equlv. of Solvent at 


Solvent Solvent ' 20* 


40 


<JO 


80 ' 


KBrtioH 2 


299*18 


22.17 


24.06 


27.17 


31.8l 


iCaBr 2 +ioH 2 


280.12 


9-37 


11 .09 


13.18 


16.01 


HBr+iolLO 


261 .09 


0.86 


8.11 


9.72 


12.15 


KBr+2oH g O 


479-3 


3-04 


3.78 


4-94 


6.75 


4CaBr ? ^2oH 9 


460.3 


1.663 


2.23 


3-19 


4-47 


HBrr2oHT) 


441 .3 


1 .312 


1.87 


2.70 


3-94 


KBrf3oH 


659.5 


1.068 


1.521 


2.24 


3.34 


iCaBr 2 r 3 oH 


640.4 


0.663 


1 .021 


1.60 


2.51 


HBrf3oH 


621 .4 


0.605 


0.913 


1.496 


2.31 



ARGEHTUM 10 

EQUILIBRIUM BETWEEN MIXJBD CRYSTALS OF SILVER 
BROMIDE AND SILVER CHLORIDE AND HALOGEN SOLUTIONS 

(Yutzy and Kolthoff, 1937.) 

The experiments were made by adding a measured volume of standard 
AgN0 3 solution to mixtures of NaCl and KCl solutions of known com- 
position. After precipitation the solutions were made up to known 
volumes and the suspensions shaken for various periods of time. The 
bromide content of the centrifuged suuernatant solution was deter- 
mined by the D'Ans and HCfer method (Z. Angew. Chem. 47 73 1934-) 
From this the ratio of Ag Br to Ag Cl in the precipitate could be 
calculated by difference. 

The results are given in terms of the mol. percent bromide in the 
precipitate and the final bromide concentration of the solution. 
By means of variation in the mode of mixing the constituents is was 
shown that equilibrium was reached in all cases. The results show 
the distribution coefficient of bromide between aq. solution and 
mixed crystals of AgCl+AgBr at 27 and at 98. 



SOLUBILITY OP SILVER BROMIDE IN LIQUID AMMONIA 

t Oms. AgBr per 100 gms. NH 3 

Q t 2.40 (Linhard and Stephan, 1933 , 1934- 

25* 5.92 (Hunt and Boncyk , 1933-) 

100 gms. liquid sulfur dioxide dissolve 0.003 Z- AgBr at o (Jander 
and Wickert, 1936; Jander and Ruppold, 1937. 



SOLUBILITY OP SILVER BROMIDE IN METHYL AND IN 
ETHYL ALCOHOL AT 25 . 

(Koch, 1930.) 

From conductivity and E.M.F. measurements the ratios of the solubilities 
of silver bromide in water and alcohols were calculated. By means of 
these figures and previously determined results for the solubility of 
silver bromide in water the following values were obtained. 

Solvent Mola. AgBr per liter Oms. AgBr per liter 

Water 7.8 x io~ 7 0.000146 

CHjOH 3.0 x io~ 8 0.0000056 

C g H 5 OH 3.7 x io~~ 9 0.00000013 

The solubility product of AgBr in CH 3 OiI at 25 in equiv. gms. per 1000 
gms. CH 3 OH is 5. 8 x io~ 16 (Buckley & Hartley, 1929.) 



SILVER BROMIDE THIOSINAMINE AgHr.NH .CS ,NHC,H K 

3 o 



II ARGENTUM 

SOLUBILITY OF SILVER BROMIDE - THIOSINAMINE 

(ALLYL THIO CARBAMIDE) IN WATER 
(Shcppard and Hudson, 1927.) 

The solutions were shaken at constant temperature for q.8 hours and 
the amount of compound dissolved determined by conversion to silver 
sulf ide. 

t AgBr.NH-.CS.NHCUi per liter sat. aq. solution 

. & 3 Q -A _ i 

' Oms. On. Mols. x 10 

IS 0.0446 1.46 

25 0.071 2.33 

35 0.121 3.94 

50 0.293 9.63 

Fusion POINT DATA FOR MIXTURES OF SILVER BROMIDE AND 
OTHER COMPOUNDS 

AgBr-AgCl (Monkemeyer, 1906.) 

AgBr-Ag I 

AgBr-AlBr (Kendall, Crittenden, and Miller, 1923.) 

AgBr-KBr 3 (Sandonnini, 1912; Zemczuzny, 1926) 

AgBr-NaBr (Sandonnini and Scarpa, 1913; Zetnczuzny, 1926.) 

AgBr-PbBr 2 (Matthes, 1911.) 

Note. Freezing or Melting Point Curves as Solubility Data. 

When a mixture of two compounds, rendered liquid by elevation of 
temperature, is gradually cooled, a point will be reached at which 
one or the other of the constituents will separate as a solid. This 
point represents the solubility of the one compound in the other. 
The method involved, differs principally from that ordinarily employed 
for solubility determinations, in that the composition of the mixture 
remains constant while the saturation temperature is being approached, 
instead of the reverse procedure. 

A considerable amount of data of this character is available but, 
after careful consideration, it has been decided that references only 
will be given to such results in the present volume, except in cases 
of mixture of well known compounds or of those in which water is one 
of the constituents. 

SILVER BROMATE AgBr0 3 . 

SOLUBILITY IN WATER. 





t. Cms. 


AgBrOa per Liter. Authority. 






2O 


1.586 (Bottger, 1903.) 






24.5 


I.9II (Noyes, 1900.) . 






25 


1.68 (Longi, 1883.) 






27 


I.yi (Whitby, 1910, see note, p. 608.) 




25 


1.949 (Hill, 1917.) 




SOLUBILITY OF SILVER BROMATE IN WATER. 






(Reedy, 1921.) 






Cms, AgllrOa 


Cms. AgUrOa f 


Cms. AgBrOj 


f. 


per JOO gins. HjO. 


t". per 100 gins. H a O. t- 


por 100 gms. H t O. 


?5 


O 1 06 


5o.. . 0.433 75 


0.832 


3o 


0.207 


5-") 0.497 80. . . . 


o.()36 


35 


, 0.269 


Go 0.570 85. ... 


. . i.o55 


Ao 


o 3i6 


65. o 648 QO. . . . 


i . 3-J.5 


45,, 


0.371 


70 O.735 





A transition point near 98. 5 is indicated. 



Vg AR6ENTUH 



12 



BrO 



SOLUBILITY OF SILVER BROMATE IN AQUEOUS ACETIC ACID AT 25. 

(Hill, 1917.) 

Cms. AgBrO, per 
Liter. 

1.863 

I.80I3 

1.6178 

SOLUBILITY OF SILVER BROMATE IN AQUEOUS AMMONIA AND NITRIC 
ACID SOLUTIONS AT 25. 

(Loagi, 1883.) 

Cms. AgBrO 3 per 



Normality of Aq. 
Acetic Acid. 

0.0498 
0.0997 
O.I99S 


Cms. AgBrOj per 
Liter. 

1.9429 

1-9379 
1.9206 


Normality of Aq. 
Acetic Acid. 

0.4988 

0-9975 
I.872I 



Solvent. 



Ammonia 
Ammonia 
Nitric Acid 



Sp. Gr. 0.998 = 5% 
Sp. Gr. 0.96 = 10% 
Sp. Gr. i. 2 1 = 35% 



1000 cc. Sol. 

35-i 
443 - 6 
3-8i 



1000 Gms. Sol. 

35-54 
462.5 
3 .12 



SOLUBILITY OF SILVER BROMATE AT 24.5 IN AQUEOUS 
SOLUTIONS *OP: 



Silver Nitrate (Noyes). 

Normal Content. Gms. per Liter. 



AgNOa. 

o.o 
0.0085 
0.0346 


AgBrO 3 : 
O.OoSl 
0.0051 
O.OO22 


AgN0 3 . 
0-0 

1-445 
5.882 


AgBrOa. 
I .911 
1.203 
0.510 



Potassium Bromate (N.). 

Normal Content. Gms. per Liter. 

'KBr0 3 . AgBr0 3 . KBrO 3 . AgBrO*. 

o.o 0.0081 o.o 1.911 

0.0085 0-00519 1-42 I-225 

0.0346 0.00227 5.78 0.536 



SOLUBILITY OF SILVER BROMATE IN AQUEOUS SALT SOLUTIONS AT 23. 
( Dalton, Poiueroy and Weymouth, 1024. ) 

Constant rotation for at least 1 6 hours was employed and equilibrium was 
approached both from above and below. 



I 
Salt. 

None i= H 2 O) . . 
KClp, 


Gm. 
equlv. salt I 
>er 1000 gms. 
JI 8 s 

o.o c 
o . 02 5 i 


)enslly 
of 
at. sol. 

9990 
OO IO 


KlUImols. 
A.gBr'0, 
per tooo gms. 
HjO. 

8.062 
8 716 


. ... 


o 5 i 


oo33 




...... 

KJ.SO, 


o. 10 
o o*>5 


.0074 

OOOC) 


9* r 9 
9-7^6 

9>fiO 




o o5 


0028 


.292 




o . to 


0062 


Ii nn*> 


MS<NO,. a 

)> . . 


o.o-j>.5 
o o5 


.0008 
0018 


8.935 

9f\ \ f\ 





O IO 


oo4.6 


.414 


MgSO 4 . 


O.O2 




8 no 





P . o5 1 
o 100 


- 


.gx 

9-67 

in ^n 





0.1088 




i i . '^ft 



Salt. 

Da (N0 a ) a 
)) 

Na, SO,, . 




Cd SO* . 



KNO a . 



Gm. 

oquiv. salt 

per JOOO gms. 

II, 0. 

O . O25 

o.o> 

0. IO 

o . o5 
o. 10 
i .00 
o. 10 
o.oo 
o . o i ^5 

. O . O25 

. 0.040 

. O.IOO 

. O . 2OO 

. 0.394 





Millimtyts. 


Density 


AffBrOa 


of 


per 1000 gms. 


sat. sol. 


H 2 0. 


.oor8 


9.088 


.0046 


9.655 


.0098 


10.873 


. oois 


9 9<>5 


.0059 


10.973 


-.0622 


18.619 


.0017 


io.4o5 


.0492 


13.349 


. 0002 


8.888 


1 .0014 


9.336 





9.12 





9-9^ 


- 


1 1. 06 


- 


12.66 



ARGENTUM 



SILVER BROMATE 



SOLUBILITY OF SILVER BROMATE IN AQUEOUS SOLUTIONS 
OF SODIUM NITRATE AND SODIUM PICRATE AT 20. 

(Gilbert, 1929.) 



Holallty of S$lt Solution 



0.00 
0.10 

0.05 



0. 10 
0.00 
0.05 



Molallty of dissolved 
AgBr0 3 

0.00848 
O.OOS^O 
0.00838 



SOLUBILITY OF SILVER BROMATE IN AQUEOUS SOLUTIONS 
OF METHYL ALCOHOL AND OF ETHYL ALCOHOL AT 25 * 

(Owen. 1933; Newman, 1934.) 



Results for Methyl Alcohol 

Wt. Percent dg g Mllllmola 
CHjOH in of per liter 

Solvent Solvent Sat. Solution 



Results for Ethyl Alcohol 



0.0 


0.9989 


8.12 


10.0 


0.9802 


5.51 


20.0 


0.9650 


3.79 


30.0 


0.9492 


2.65 


40.0 


0.9318 


1.82 


50.0 


0.9123 


1.24 


60.0 


0.8908 


0.83 



It. percent 


d25 


Mllllmola j 


CoK s OH 


of 


per lit* 


In Solvent 


Solvent 


Sat. Solu 1 


0.0 


0.9989 


8.12 


10.0 


0.9804 


5-53 


20.0 


0.9664 


3*86 


30.0 


0.9507 


2.78 


40.0 


0.9315 


1.97 


50.0 


0.9099 


1.36 



SOLUBILITY OF SILVER BROMATB IN AQUEOUS SOLUTIONS 
n PROPYL ALCOHOL AND IN |so PROPYL ALCOHOL AT 25- 

(Owen. 1933; Newman, 1934.) 



Results for n Propyl Alcohol 
Wt. Percent dps Ml Illinois AgBrOg 



In Solvent 


~sr> 
Of 

Solvent 


per liter 
Sat. Solution 


10 
20 


0.9821 
0.9674 


5.80 
4.36 


30 
40 
50 


0.9472 
0.926l 
0.9051 


3.31 
2.41 
1.63 



Results for ls.0. Propyl Alcohol 
Wt. percent Mllllmola 

(CN 3 )s>CHOH 
in Solvent 



per liter 
Sat. Solution 



10 

20 

30 
40 

50 



5-5 

3-95 

2.92 

2.1 

1-5 



BrO 



SOLUBILITY OF SILVER BROMATE IN AQUEOUS SOLUTIONS 
OP ACETONE, MANNITOL AND GLYCINE AT 25. 

(Owen. 1933.) 



Wt. Percent 

Organic Cmpd. 

In Solvent 



5 

10 
15 

20 
30 
40 



In Acetone In Mannltol 
dgs of Mllllmola AgBrOg d ?<5 of Mllllmola Agf 
aq. per liter aq. per liter 
Acetone Sat. Sol. Mannltol Sat. Sol. 


0.9845 5-92 


1.0147 
1.0328 
1.0513 


8.24 ' 
8.38 
8.51 



0.9700 
0.9537 
0.9355 



4.29 
3.OO 
2.03 



In Olyclne 
dj>5 Of Mllllraols AgBrOS 



aq. 
Olyclne 



i .0184 
1.0395 
1 .0613 



per liter 
Sat. Sol. 



12.9 
18.4 
24.9 



g ARGEHTUM 

SILVER BROMATE AgBr0 3 



SOLUBILITY OF SILVER BROMATE IN AQUEOUS SOLUTIONS 
OF ETHYLENE GLYCOL AND OF GLYCEROL AT 25. 

(Owen, 1933.) 



Results for Ethylene Glycol 



't. Percent 


das of 


Mlllimols AgBrO.-} 


ICH & .CH20H 


aq. 


per liter 


in Solvent 


Solvent 


Sat. Sol. 


10 


1 .0097 


7.26 


20 


1 . 0228 


6.50 


30 


1.0362 


5.85 


40 


1.0496 


5.26 


50 


1.0624 


4.70 


70 


1.0851 


3.6l 



:H 



SILVER METHIONATE 



25 

25 



Results for Glycerol 

Wt. Percent dp= of 
OHCHoCHOHCH 2 OH aq. 
In Solvent Solvent 



Mlllimols AgBrOs 
per liter 
Sat. Sol. 



10 


1 .0207 


7.80 


20 


l. Oil 53 


7.49 


30 


l .0706 


7-15 


40 


1 .0971 


6.8q 


50 


1.1239 


6.48 


60 


l .1511 


6.08 


70 


1.178*1 


5-59 


80 


1.2054 


. 4-94 



SOLUBILITY IN WATER 

(Backer and Terpstra, 1929.) 



per 100 gns. Hio 

62.5 
45-05 



Solid 
Phase 



SILVER ACETATE CH 3 COOAg. 

SOLUBILITY IN WATER. 

(Xcrast, 1889; Arrhenius, 1893; Goldschmidt, 1898; Nauman and Rucker 1905: Raupenstrauch , 
1885; Wright and Thompson, 1884, 1885.) 



Gms.Ag(C 2 H 3 O 2 ) 
per Liter. 



O 

10 



25 
30 
40 



per Later. 
II. 2 
12. 1 



20 



t fa . 


Cms. Ag(C 2 H 3 O 2 ) 
per Liter. 


50 
60 


16.4 
18.9 


70 
80 


21.8 
25 -2 


S 10, 


.03 gins. AgCH 3 COO 



7 .22 

8-75 
9.4 

10.4 

At 18 one liter sat. solution in water contains 10.03 
(Larsson and Adell, 1931). 

At 25 one liter sat. solution in water contains 11.07 gms. AgCiUCOO 
(Ja^ties, 1909); 11.13 g*ns. (Hill and Simmons, 1909); (Knox and'Will, 1919); 
11.09 gs, d 25 sat. sol. = 1.0047 (MacDongall, 1930; MacDougall and 
Kehner, 1934; MacDougall and Bar tsch, 1936; MacDougall and Larson, 1937). 

SOLUBILITY OP SILVER ACETATE AT 18 IN AQUEOUS SOLUTIONS OF: 

fLarsson and Adell, 1931.) 



Sodium Hit rate 
ttolea per liter Sat. Sol. 



o.o 


0.060 I 


O.2 


0.0686 


O.4 


0.0734 


0.6 
0.8 


0.0767 
0.0790 


1,0 


0.0810 



Sodium Acetate 
Moles per liter Sac. Sol. 



; NttCHgCOO 


AgCH 3 COO A 


0.0503 


0.0429 


0.1005 


0.0317 


0.2011 


0.0223 


0.2513 


0.0211 


0.503 


0.0153 


1.005 


0.0121 



ARGEHTUM Ag 



SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF: 



Silver Nitrate. 



Gms. 
AgN0 3 
per Liter. 


Gms. CH 3 COOAg per Liter at: 


if>(Nernst). 


1 9 .8 ( Arrhenius) . 





10.05 


9-85 


5 
10 


8.2 

7-o 

6.4 


7-9 
6.6 

5-5 


2O 


5-7 


4-5 


30 


4-4 




40 


3- 2 





Sodium Acetate. 



^V./VJT' 

r Liter 
O 

5 

10 


. 16 (N.,N.andR.). 
10.05 

6-3 
4 .6 


9-9 
6.6 
4.9 


15 


3-8 


4.1 


20 

30 


3-3 


3-5 

2.8 


40 




2.4 



SOLUBILITY OF SILVER ACETATE IN AQUEOUS SALT SOLUTIONS AT 25. (jaques, 1910.) 



Aq. Solution of; 

Water alone 
Cadmium Acetate 



Lead Acetate 



Gms. Salt. 
per Liter. 


Gms. 

AgC 2 H q 2 
per Liter. 





II. 08 


I . 15 


10.39 


5-76 


8.10 


11.52 


6.71 


57-6 


4-33 


II5.2 


3-95 


1-63 


10.69 


8.13 


9-45 


16.26 


8-34 


81 .3 


7.26 


162.6 


5-99 



Aq. Solution of: 

Potassium Acetate 



Silver Nitrate 



Sodium Acetate 



Cms. Salt 
per Liter. 


pefler 2 


2.22 


9.60 


22.2 


4-43 


III 

222 


2.41 
2.18 


2.77 


9-93 


5-55 


9 


II. 10 
22.21 


7.41 

5-81 


1.97 


9.27 


19.7 

98.5 


4.21 
2-33 


197 


2.07 



SOLUBILITY OF SILVER ACETATB IN AQUEOUS SOLUTIONS 

OP POTASSIUM NITRATE AT 25. 

(rtacoougaii. 1930). 



ID 


d 2S of 


m 


c 




m 


d2S of 




m 


c 


KNOs 


Sat. Sol. 


AgCH 3 COO 


AgCHgCOO 




KNOfl 


Sat. Sol. 


AgCHgCOO 


AgCHsCOO 


0.05O1 


1 


.0077 





.06685 


0.06642 





.8021 


1.0537 


0. 


08786 


0.08449 


0.1006 


1 


.0115 





.07281 


O.O7204 


1 


.0155 


1.0658 


0. 


09019 


0.08600 


O.2O01 


1- 


.Ol8o 


O 


.07659 


0.07547 


1 


.2431 


1.0784 


0. 


09214 


0.08708 


O.3018 


1 


.0241 





.07941 


0.07791 


1 


5437 


1 .0944 


0. 


09453 


0.08828 


0.4010 


1 


.0298 


o 


."OSl 7 1 


0.07982 


2 


.0371 


J.1186 


0. 


09754 


0.08923 


0.5013 


1 


.0366 





.08344 


0.08124 


2 


5355 


1 . 1426 


0. 


09997 


0.08973 


0.6040 


1 


.0417 





.08498 


0.08233 


3 


.0139 


1.1653 


0. 


10163 


0.08960 



m = molality or moles of AgCi^COO per 1000 gins, of water, 
c = molarity or moles of AgCiI 3 COO per 1000 cc. of solution. 



ARGENTUM x6 

SILVER ACETATE, AgCllgCOO 
SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF NITRATES AT 25. 

(MacDougall and Rehner, Jr., 1034.) 
In Aqueous Lithium Nitrate In Aqueous Sodium Nitrate 



d?5 f Sat. 


Moles per 


l00 gms Hgo 


Solution 


L1N0 3 


AgCKsCOO" 


1 .0050 


0.0 


0.06666 


1 .0067 


0.04817 


0.07033 


1 .0097 


0.0994 


0.07280 


1.0143 


0.1996 


0.07799 


1 .0185 


0.2997 


o.o8j 98 


1 .0226 


0.4002 


0.08490 


1 .0269 


0.5004 


0.08765 


1.0314 


0.6l01 


0.09033 


1 -0395 


0.8195 


0.09491 


1 .0461 


0.9975 


0.09819 


l .0561 


1 .2636 


0.1031 


1 .0649 


1 -4997 


0.1072 


1.0925 


2.2835 


0.1195 


1.1002 


2.5193 


0.1229 


1 .1172 


3.0305 


0.1315 


1 .1444 


4.0221 


0.1479 


1 .2050 


6.0125 


0.1851 


1 .2560 


8.0153 


0.2274 


1.3007 


10.055 


0.2768 


In Aqueous Calcium Nitrate 


dps of Sat. 


Moles per 


100 gms. Hgo 


Solution 


' Ca(N0 3 )z 


AgCH 3 COO ' 


l .0062 


0.00499 


0.06825 


l .0071 


0.00993 


0.06920 


l .008*1 


0.01996 


0.07187 


1 .0126 


0.04980 


0.07691 


l .0191 


O.0997O 


0.08365 


l .0318 


0.1996 


0.093H 


1 .0560 


0.3985 


0.1067 


1.0792 


0.5985 


0.1170 


1 .1225 


0.9962 


0.1363 


1 .1726 


1 .4916 


0.1538 


1.2634 


2.4958 


0.2034 


1.3766 


3.9871 


0.2759 


In Aqueous Barium 


Nitrate 


aj>5 or Sat 


Moles per 


10^0 gjns. H?o 


Solution 


'Ra(N0 3 ) 2 


AgCHsCOO " 


1 .0050 


0.0 


0.06666 


1 .0064 


0.005012 


0.06796 


1.0076 


0.01001 


o .06910 


1 .0100 


0.01998 


0.07127 


1 .0161 


0.05025 


0.07597 


1.0273 


O.I 002 


0.08104 


1 .0489 


0.2009 


0.08831 


1 .0697 


0.3014 


0.09361 


1 .0796 


0.3500 


0.09572 


1.0876 


0.3902 


0.09755 



d?5 of at. 
Solution 

1 .0086 
1 .0108 
l .0162 
1 .0216 
1 .0269 
1 .031u 
1 .0371 
1 .0470 
l .0578 
0629 
0718 
0857 
1038 
1246 
1458 
1846 
2628 
3212 

3753 



Moles per IpOO gms^H^ 

AgCHgCOcP 



NaNO ? 
0.0/1776 

0.1914 
0.2868 
0.3840 
0.4707 
0.5743 
0.7631" 
0.9533 
l .0504 
1.2398 
1.5325 
l .9108 
2.3884 
2.8723 
3-9954 
6.0191 
8.0098 
10.225 



0.070<fO 

0.07287 
0.07640 
0.08032 
0.08246 
0.0841^ 
0.08615 
0.08910 
0.09177 
0.09266 

0.0940't 

0.09766 

0.09958 

0.1027 

0.1059 

0.1 1 06 

0.113 

0.1123 

0.1109 



In Aqueous Strontium Nitrate 



dgs of Sat. 
Solution 



Moles per IjpOO gms. HgQ 



.0063 
.0071 
.0090 
.0134 
.0229 
.0402 



1.0727 



1 ,1046 
l .1645 
1.2338 
1.3575 
l .4605 



(Sr(N0 3 ) 2 

0.00497 

0.01001 

0.02002 

0.05038 

0.1008 

0.2009 

0.4022 

0.6036 

1 .0064 

1 .5072 

2.5092 

3.4941 



AgQfeCOCT 

0.06768 

0.06870 

0.07133 

0.07628 

0.08178 

0.03936 

0.1001 

0.1081 

0.1218 

0.1354 

0.1588 
0.1632 



In Aqueous Lanthanum Nitrate 



dg5 of Sat. 
Solution 

1 .0060 
1.0073 
l .0085 
1 .0122 
1 .0228 
1 .0389 
I .0715 
1 .1210 
1 .l6l3 
1.2558 
1.4571 
1 .6277 



Moles per ffQO gms. Hpo 



' La (N0 3 ) 3 

0.001431 

0.004859 

0.008374 

0.01839 

0.05047 



0.2113 
0.3908 
0.5434 
0.9216 
1.8568 
2.8l85 



AgCH;,COO 

0.46809 
0.07109 
0.07*107 
0.08231 

0.1034 

0.1304. 

0.2315 
0.2771 

0.3856 

0.6764 
1.0*187 



ARGENTUM 



SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT 25. 

(Hill and Simmons, 1909.) 

Gms. AgCsHA 
per Liter Sat. Sol. 

11.13 

85-3I 
161.9 

307-4 

549-3 
656 
792.2 
Results are also given f ortne solubility of AgCjHiOa-f- AgN0 3 in Aq. H NO 8 at 25. 

SOLUBILITY OF SILVER ACETATE, IN AQUEOUS SOLUTIONS or ACETIC ACID AT 25. 

(Knox and Will, 1019.) 
Saturation was secured by constant agitation in a thermostat. 

equlv. CH 3 OOOir 
per liter. 

12.32 



Normality of 
Aq. HN0 3 : 


Per cent HN0 3 in 
Solvent. 


d* of 
Sat. Sol. 


O 





1.005 


0.50 


3.096 


1.072 


I 


6.128 


I.I40 


2 


n-757 


I .267 


4.O2 


22.386 


1.470 


5-03 


27.328 


1.561 


6.44 


33-8j:3 


1.670 



Gm. 


Gins. 


IT. CH a COOII 


CH S COOA 


per liter. 


per liter. 


O.O 


ii. i3 


I . OO 


10.73 


2 . 00 


1 O. 32 


2.98 


9.98 


4-i9 


9.52 


4.98 


9- '9 



Gm. 


Gms. 


equlv. CHjCOOK 


cn 3 coo AS 


por liter. 


per liter. 


5-99 


8.7* 


6.80 


8.29 


8.01 


7.73 


8.97 


7 .3i 


9-96 


6.78 


I I . 02 


6.i5 



1^-97 
i3. 97 
14.96 
i5. 9 3 

1 7 . 28 



Cms. 

CIf 3 COO \g 
per liter. 

5 33 

4.96 
4.29 
3.43 
2.48 
i .09 



too gms. sat. solution of silver acetate in acetic acid contain 0.09/1 g m - CII 8 CO Ag 
at 76 and O.2O4 gm. at Il5. (Kendall and Adler, 1921.) 

SOLUBILITY OP SILVER ACETATE IN AQUEOUS SOLUTIONS 

OK &THYL ALCOHOL AT 25. CH 

(MacDougall and Bartsctt, 193e.) 



Wt. Percent d 25 Holes AgCHsCOO 

C 2 H 5 OH in of per 11 tar 

Sat. Sol. Sat. Sol. 



C ? H 5 OH in 
Solvent 



percent <l S Moles AgC%COO 

HsOH in of per liter 

olvent Sat. Sol. Sac. Sol. 



5-0 

7.62 

9.0 

15.03 

19.96 



0.9955 
0.9898 
0.9882 
0.9784 
0.9696 



0.0577 
0.0523 
0.0506 
0.0413 
0.03 



25.06 
29.82 
30.05 
40.27 
50.14 



0.9616 
0-9530 
0.9926 
0.9323 
0.9102 



O.O294 
0.0251 
0.0249 
0.0180 
0.0124 



Results are also given for the solubility at 25 of silver acetate in 
approximately 10, 20 and 30 percent aqueous ethyl alcohol mixtures con- 
taining varying concentrations of KN0 3 , NaN0 3 , LiN0 3 , Ca(N0 3 )j,, Sr(N0 3 ) g 



and Ba(N0 3 ) 2 . 



SOLUBILITY OP SILVER ACETATR IN AQUEOUS SOLUTIONS 
OF ACETONE AT 25. 

(rtacl)ougall and Larson, 1337.) 



t. Percent 
CHsigCO In 


%> 


Moles AgCH^COO 
per liter 


Solvent 


Sat. Sol. 


Sat. Sol. 


9.27 


0.9920 


0.0516 


9.Bl 


0.9910 


0.0499 


10.35 


0.9900 


0.0481 


18.83 


0.9758 


0.0324 


19.48 


0.9748 


0.0323 



We. Percent 
(CHsJgCO In 


doe Moles AgCH-rCOO 
oT per liter 


Solvent 


Sat. Sol. 


Sac. Sol. 


20.03 


0.9740 


0.0322 


20.50 


0.9724 


0.0319 


28.25 


0.9592 


0.0214 


20.23 


0.95B4 


0.0213 


30.02 


0.95^4 


0.0213 



Results are also given for the solubility at 25 of silver acetate in 
approximately 10, 20 and 30 percent aqueous acetone mixtures containing 
varying concentrations of KN0 3 , NaN0 3 , 3r<N0 3 ) 2 and Ca(N0 3 ) a . 



Ag ARGENTUM l8 

SILVER ACETATE AgCH g COO. 

SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OF SEVERAL 

COMPOUNDS AT 25. (Armstrong and Eyre, 1913.) 



Aqueous 
Solution of: 


Grns. 
Compound 
per 
looo Gms. 

TT f\ 


Gms. 
AgC s H 3 2 
per looo 
Gms. 


Aqueous 
Solution of: 


Grns. 
Compound 
per 
1000 Gms. 


Gms. 

per 1000 
Gms 


Water 

Acetaldehyde 
Paraldehyde 


H 2 O. 
O 
II 
II 


Sat. Sol. 
II. 08 
10.13 
8.92 


Propyl Alcohol 

H il 

Glycerol 


H 2 O. 

15 
60 

9-21 


Sat. Sol. 
9.88 
8.03 

8.66 


Isobutyl Alcohol 


33 
66.4 


9.l6 

7-55 


Glycol 

u 


I 5-5 
62.1 


10.86 
8.44 



^AUKH fionochloi 


" ACETATE 


AgCHgCICOO. 






16 9 6 ll (A 6r aque us ( 501 - ull0ri contains 12.97 gms. AgCH ClCOO at 


SOLUBILITY op 


SILVER MONO CHLOR ACETATE AT 16 o 
AQUEOUS SOLUTIONS OF: 


IN 


Silver Nitrate. 

' _^ "^~~ N. 


Sodium Chlor Acetate. 


Gms. 
AgNC) 3 
per Liter. 


Gms. 
CH 2 ClCOOAg 
per Liter. 


Gms. 
CH 2 ClCOONa 
per Liter. 


Gms. 
CH 2 ClCOOAg 
per Liter. 




O -O 
f\ f\ 


I2. 97 


0.0 


12 .97 




9.0 
17.0 


10.05 

7-55 


3-88 

7-77 


10.05 
8.16 








15 -53 


6 .02 








31-07 


4.19 








58.26 


3.26 




SOLUBILITY OF SILVER 
SOLUTIONS op 


MONO CULOR ACETATB 

BARIUM NITRATB AT 


IN AQUBOUS 
25. 






(MacDougaii 


and Rehner. jr., 1934.) 






*& of Noles per 1000 BUS. H.O 


d ?5 of 
Sat. Sol. 


Moles per 1000 gros. H p O 


AC. soi. ^wy? 




Ba(N0 3 ) g 


AgCHgClCOO " 


1 . 0097 . 
1-0100 0.00493 


0.07832 


.0319 


0.09916 


0.09493 


1-0114 0.00987 
1.0136 0.0199O 
1.0207 0.05000 


0.08180 
0.08340 
0.08878 


0535 
.0739 
.0846 
.0922 


O.20O1 
0.2980 
0-3501 
0.3871 


0.1035 
0.1099 
0.1131 
0.1151 



- 



ARGENTUM Ag 



SILVER Monochlor ACETATE AgClIgClCOO 



SOLUBILITY OF SILVER MONOCHLOR ACETATE IN AQUEOUS SOLUTIONS 
OF NITRATES AT 25. 

(MacDoufsall and Rehner, Jr., 1934.) 



In Aqueous Lithium Nitrate 



In Aqueous Sodium Nitrate 



d 
Sat 


25 f 
. Sol. 


Moles per ia 


uu gms. Hp(j 


Q 25 of 
Sat. Sol 


r 


mica per iuuu 


STO 


"20 


' LiNOg 


AgCh?ClCOO x 


' NaWOjs AgCHgClCOO^ 


1 


.0123 


0.05039 


0.08199 


1 .0125 


0.04979 


0. 


08004 


1 


.0191 


0.2001 


0.09026 


1 .0219 


0.1994 


0. 


08923 


1 


.0277 


0.4004 


0.09772 


1.0334 


0.3990 


0. 


096l7 


1 


.0440 


0.8081 


O.lOSl 


1.0555 


0.7975 


0. 


1059 


1 


.0696 


1.5025 


0.1186 


l .0907 


1 


4930 


0. 


1170 


1 


.1210 


2.9908 


0.1436 


1.1583 


2.9847 


0. 


1320 


1 


.2079 


6.0071 


0.1648 


1.3793 


9 


.9368 


0. 


1568 




In 


Aqueous Potassium 


Nitrate 


In 


Aqueous 


Calcium Nitrate 


dge^-of Moles per 1000 gms. H?o 


Q 25 of 


lOOOMoles per 1$>00 gms 


s. H ?0 


Sat. Sol. 


' LiN0 3 


ACH 2 C1COO\ 


Sat. Sol 


. ' C 








1 


.0127 


0.05005 


0.08306 


l .0102 





.00*199 


0. 


O8ll8 


1 


.O229 


0.1999 


0.09H2 


.0127 





.01996 


0. 


08503 


1 


.0353 


0.3971 


0.09825 


.0363 


O 


.1996 


0. 


1063 


1 


.0598 


0.7980 


0.1087 


.0611 





.3985 


0. 


1208 


1 


.0851 


1.2464 


0-.1183 


.1066 





.7958 


0. 


14-12 


1 


.1244 


1.9923 


0.1316 


.1782 


1 


.4916 


O. 


1728 


1 


.172*8 


2.9960 


0.1440 


1.3786 


3 


.9B71 


o. 


2550 




In 


Aqueous Strontium 


Nitrate 


in 


Aqueous 


Lanthanum Nitrate 


^25 Of 


Moles per 1000 gms. Hj>0 


d 2S of 


Moles per IpjDO 


gms. Hpo 


Sat. Sol. 


/ Sr(N0 3 )2 


AgCHpClCOO^ 


Sat. Sol 


1 La(N0 3 ) ? AggCHyClCOC^ 


l 


.0100 


0.004978 


0.08139 


1.0103 





.001431 


0.8211 


1 


.0133 


0.01983 


0.08466 


1 .0129 





.008374 


0.08680 


1 


.0279 


0.09998 


0.09524 


1.0268 





.05047 


0.1080 


l 


.0452 


0.1989 


0.1044 


1.0752 





.2113 


0.1569 


1 


.0786 


0.3992 


0.1175 


1 . 1226 





.3908 


0.1879 


l 


.1103 


0.0008 


0.1274 


1 .2098 





.7371 


0.2441 


1 


.1407 


0.7993 


0.1362 


1.3149 


1 


.2013 


0.3164 


J 


.2394 


1 .4977 


O.l6o6 


1.4465 


1 


.8568 


0.4237 


1 


.4180 


2.9985 


0.1975 


l .6080 


2 


.8185 


0.5939 


SOLUBILITY OF SILVER MONOCHLORO 


ACETATE IN NITRIC ACID AT 


25 6 . 


(Hill and Simmons, 1909-) 






Normality 
of Aq. 
HNOj. 


Gms. HNO 3 
per zoo Gms. 
Solvent. 


Sat! Sol. 




Gms. 
AgC 2 H 2 C10 2 
per Liter. 










O 


C 


1.0095 




I5.l8 










0.25 


1.564 


1.0426 




50-33 










0.50 


3.096 


I.079I 




91.83 










I 


6.128 


I-I473 




167-3 










2 


n-757 


1.2716 




310.8 










4 


22.277 


1.4749 




549-1 










5 


27-185 


I-5673 




659.2 







CH 



ARGENTUM 20 

SILVER Dipropyl ACETATE AgGH 15 2 . 

ioo gms. H 2 O dissolve 0.123 gm. AgC 8 Hi 5 O2 at 11.7, and 0.190 gm. at 72. 

(Fiirth, 1888.) 

SILVER Methyl Ethyl ACETATE Ag.CH 3 .CH 2 CH(CH 3 )COO. 
SILVER Diethyl ACETATE Ag[(CiH)iCH.COO]. 
SILVER Trimethyl ACETATE Ag(CH 3 ) 3 CCOO.* 

SOLUBILITY OF EACH IN WATER. 

(Sedlitzky, 1887; Keppish, 1888; Stiassny, 1891.) 



Cms, per ioo Gms. HjO. 



Gms. per ioo Gms. H 2 O. 





Ag.QHA. 


AgCeHuCX. 


AgCsHA-* 


t . 


AgC 5 H 9 2 . 


AgQHnOj. 


AgCsHA-.* 





1. 112 


O.4O2 


I.IO 


50 


I. 602 


0-536 


i-47 


ID 


I.I26 


0.413 


I-I5- 


60 


1.827 


0.585 


i .57 


20 


I.I82 


0.432 


1.22 


70 


2.093 


0.643 


1.68 


30 


1.280 


0.458 


1.22 


80 


2.402 




i. 80 



SILFEM Ptieayl ACETATE AgC 6 H 5 CH 2 COO 

ioo cc. sat. solution in water contain 0.352 gm. 
SILVER PROPIONATE C,H 5 COOAg. 



? .C 6 H C11 2 COO at 25. 
i Larson , 1927 .) 



f. 

o 

10 

18.2 



SOLUBILITY IN WATER. 

(Raupenstraudi, 1885; Arrhcnius, 1893; Goldschmidt, 1898.) 



S- 

' 7 , ,. 
8 -36 (A) 



20 
25 



8.36(8.48) 

9.06 

9.93(9.70) 



50 
7 o 
80 



Gms. C a H 8 OjAg 
per Liter. 

13-35 
17.64 
20.30 



ioo cc. sat. solution in 11^0 contain 0.9 gm. AgC ? (l s COO at 25. 

( Larson , 1927 . J 
ioo cc. sat. solution in H ? contain 1.353 gm. AgC ? M 5 COO at 50. 

(Fuhner, 1924. J 
SOLUBILITY OF SILVER PROPIONATE IN AQUEOUS SOLUTIONS OF: 

(Arrhenius.) 
Silver Nitrate at I9 . 7 . Sodium Propionate at 18.='. 

Mols. per Liter. ~ 





^ ^^_ -, ^ uie r. Mob. oer Liter. r.. M , r u .. 


AgiMUj. 
O 
0.0133 
0.0267 

0-0533 
0.100 


0.0471 
0.0415 
0.0379 
0.0307 
0.0222 


AgNO,. 

2.289 
4.577 
9.059 
16.997 


8 

7 
6. 

5- 
4. 


IAAg. 
519 
511 
.86 
556 
019 


C',HjO,Na. C a H,OjAg. 

o 0.0462 

0.0167 0.0393 
0.0333 0.0345 
0.0667 0.0258 
- I 333 0.0191 


C 3 H 6 0,Na. 
O 
1.607 
3.215 
6.429 
12.859 


8. 

7- 
6. 

4. 
3- 


362 
114 
244 
670 
456 


















0.2667 0.0131 


25.718 


2. 


371 


















0.5000 o.oioi 


48.77 


I. 


828 




SOLUBILITY OF SILVER PROPIO 

r. 


NATE 11 


* AQUEOUS SOLUTIONS OF PROPIONIC A 










j 


LT: 


20. ( K 


nox and "Will, 1919 ) 










SM c^esb,, 

per liler. per liter. 
0.00 Q.4 


Gm. equlv. 

c,H s coon 

per lUer. 


/ 
Gm. 
f C^H.COOAg 
per liter. 


Gin. equlv. 
C, S COOII 
per liter. 


Cms. 
per lller. 


I. 


OO 


.7 

8 


.58 






4 ^5 


7.60 

6Q 


8.56 




4 


.96 


2. 


OO 


8 


.01 






6/\A 


.78 


1 1 . 4o 




3 


. 1 6 














. yo 


5.78 


i3.o3 




3 


*7 



21 



ARGENTUM 



SILVER Acetal PROPIONATE (.LEVULINATE) Ag .CH 3 COCil 2 CH 2 COO. 
SOLUBILITY IN WATER. 

(Furcht and Lieben, 1909.) 
f.o Gms. per 100 Gms. Sat. Solution. 

8 0.5363 (white salt) 0.5195 (yellow salt) 

9 0.5166 0.5372 
14-15 0.6078 " 0.6448 " 
99.6 3.49 3.70 

SILVER BUTYRATE C 3 H 7 COOAg. 

SILVER (Iso)BUTYRATE (CH 3 ) 2 CHCOOAg. 

SOLUBILITY OF EACH SEPARATELY IN WATER. 

(Ooldschmlcit, 1898; Arrtienlus. 1803; Raupenstrauch, 1885, Ftihner, 1924.) 



Cms. per 100 Gms. H 2 O. 



Grns. per 100 Gms. H 2 0. 



L . 


t ' 

Butyrate. 


' Iso Butyrate. 


\> . 


r 

Butyrate. 


Iso Butyrate. 





0.363 


0.796 


30 


0.561 


1. 060 


(1.1022) 


IO 


0.419 


0.874 


40 


0.647 


I.I76 


(R.) 


17.8 


0.432 (A.) 




50 


0.742 


I-3I3 




18.8 


0.445 (A.) 




60 


0.848 






20 


0.484 


0.961 (0.9986) 


70 


0.964 


I .670 




25 




... (1.0442) 


80 


I.I4 


1.898 





SOLUBILITY OF SILVER BUTYRATE IN AQ. SOLUTIONS OF SILVER ACETATE, 
SILVER NITRATE AND OF SODIUM BUTYRATE. 



(Arrhenius, 1893.) 



In Silver Acetate at 17.8. 

G. Mols. per Liter. ' Grams per Liter. 



In Silver Nitrate at 18.8. 

G. Mols.jper Liter. Grams per Liter ^ 



CHa 
COOAg. 


C 3 H 7 
COOAg. 


CH 3 
COOAg. 


C 3 H 7 ' 
COOAg. 


AgNO 3 . 


C 3 H 7 
COOAg. 


AgN0 3 . 


COOAg. 


0-O 





.0221 


o.o 


4 


32 





.0 


O.O228 


O 


O 


4-445 


O.O270 


o 


.0139 


4-5* 


2 


7* 


O 


.0667 


0.0078 


II 


33 


1 .521 


0-0506 


o 


.0103 


8-45 


2 


.01 





.100 


O.OO62 


17 


.00 


1 .209 



In Sodium Butyrate at 18.2. 



G. Mols. per Liter. 



Grams per Liter. 



G. Mols. per liter- 



Grams per Liter. 



COONa. 


C 3 H 7 
COOAg. 


' C 3 H 7 
COONa. 


C 3 H 7 ' 
COOAg. 


* C 3 H 7 
COONa. 


C 3 H 7 
COOAg. 


' C 3 H T 
COONa. 


CaH 7 
COOAg. 


o.o 





.0224 





.0 


4 


.363 


O 


.0658 


O.OO9I 


7.24 


1-774 


o . 0066 


O 


.0199 


O 


73 


3 


.881 





1315 


O.O06O 


14-47 


1.170 


0.0164 


O 


.0169 


I 


.81 


3 


.296 





.263 


O.OO4O 


28 .-96 


0.780 


0.0329 


O 


.0131 


3 


.62 


2 


555 


O 


493 


O-O027 


54.28 


0.526 



SILVER FUMARATE C 4 H 2 O 4 Ag a 

100 gms H 2 dissolve 0.018 gm. silver fumarate at 3o. (Weiss and Downs, 1023. 

SILVER MALEATE C^HsO^Ag^ 

100 gms. H 2 dissolve 0.12 gm. silver maleate at 3o. (Weiss and Downs, 1023.) 



Ag ARGENTUM 22 

SILVER MALATE C.E.0 6 Ag 2 . 

ioo gms. H 2 dissolve 0.0119 gms. at 18. and 0.1216 gm. at 25. 

(Partheil and Hiibner, 1903. 

SILVER TARTBATE CJ^OAga. 

100 gms. H 2 dissolve 0.2012 gm. C^OeAg- at 18, and 0.2031 gm. at 25. 

(Partheil and Hiibner, 1903.) 

SOLUBILITY OF SILVER TAR.TRATE IN WATER AND IN AQUEOUS SOLUTIONS OF 
BORIC ACID AT 18. ( Kolthoff, 1926. ) 

Normality of sat. sol. Gms. CJ^O u As s 

Solvent. in A ions. per liter. 

Water 0.0086 1.42 

Af. o.i rool. H 3 B0 3 .... o. 00148 (?) 2.45(?) 

o.5 o.o4i4 6.87 

The above gram quantities were calculated by multiplying the normality of 
Ag i0n by one-half the molecular weight of silver tartrate. 



SILVER SUCCINATE 

CH ioo gms. H 2 dissolve 0.0176 gm. at 18, and 0.0199 gnr at 25. 

(PartheU and Hiibner, 1903.) 



SILVER p Methyl ADIPATE (Neutral Salt). 

ioo cc. sat. solution of silver (3 methyl adipate in water contain 0.12 gm. of the 
compound at 20. (Meurisse.) 



SILVER VALERATES AgC 6 H 9 O 2 . 

Normal Valerate, CH 3 (CH 2 )a.COOAg. Iso Valerate, CH3.CH(CH 3 ) 2 CH 2 COOAg. 

SOLUBILITY OF EACH SEPARATELY IN WATER. 
(Forth, 1888; Sedlitzky, 1887.) 



to 


Gms. per ioo Gms. HaO. 




Gms. per ioo Gms. H2O. 


. 


Normal V. 


IsoV. 


t. 


formal V. 


IsoV. 


o 


0.229 


0.177 


So 


0.474 


0.360 


10 


0.259 


O.2II 


60 


O'SS^ 


O.4OI 


20 


0.300 


0-246 


70 


0-636 


0-443 


30 


0-349 


0-283 


80 




o ; 486 


40 


0.408 


0.321 









loo gms. H 2 O dissolve 0.73 gm. silver valerate at 20. (Markwald, 1899.) 

ioo cc. sat. aq. solution contains 0.71 gm. dextro silver valerate at 15. 

(Taverne, 1900.) 

ioo gms. H 2 dissolve 0.476 gms. n CH 3 (CH 2 ) 3 COOAg at 50. 

(Fuhner , 1924. ) 



ARQENTUM 



SOLUBILITY OF SILVER VALERATE IN AQUEOUS SOLUTIONS OF SILVER 
ACETATE, SILVER NITRATE AND OF SODIUM VALERATE. 

(Arrhenius, 1893.) 



In Silver Acetate at 17.8. 

Mols. per Liter. Gms. per Liter. 



In Silver Nitrate at 16.5. 

Mols. per Liter. Gms. per Liter. 



C 2 H 3 2 Ag. 

0.0067 


C 5 H fl 2 Ag/ 
0.0094 
0.0070 


QH 3 2 Ag. C & H, 
I. 

I.I3 I- 


, 9 6 
, 4 6 


'AgNOs. 
O 

0.0067 


0.0094 
o . 0068 


AgN0 3 . 
O 
I.I4 


CsHAAg. 
1.96 
1.42 


0. 
O. 
O. 


oi35 
0270 

0505 


0.0057 
0.0037 
0.00265 


2.27 

4-54 
8.48 


I. 
O, 
0. 


,19 

77 
53 


O. 
0, 
0, 


0133 

.0267 

.1000 


0. 
0. 

o. 


,0051 
,0031 

,0012 


2.29 
4.58 


1.07 
0.65 
0.25 


In Sodium Valerate at 18.6. 






Mols. 


per Liter. 


Gms. per Liter. 


O 
0.0175 
0.0349 
0.0698 


C fi H 9 2 Ag. 
0.0095 
0.0047 
0.0030 
O.OOlS 


o 

2. 

4- 
8. 


,17 
32 

65 




CfiHgOoAg. 

1.986 
0.982 
0.627 
0.376 








0.1395 


0. 


0015 






17- 


31 




0.313 





SILVER CAPROATES Ag(C 8 H n 02). (Silver hexanoates) 
SOLUBILITY OF EACH SEPARATELY IN WATER. 

(Keppish, 1888; -Stiassny, 1891; Kulisch, 1893; KQnig, 1894; Altschul, 1896.) 

Results in terms of gms. salt per 100 gms. HzO. 



2 Methyl Pentan Methyl 3 Pentan 4 Methyl Pentan 
. _ Normal Caproate 4 Acid Acid 4 4 Acid 
t. CHaCCHaUIOOAjj. CH 3 .CH.CH 3 CH 3 .CH 2 CH 3 (CH 2 ) 2 CH(CH 3 ) 






.(C 


H 2 )2COUAg. .LIU 






O 


0.076 


(A-) 0.078 (Keppish) 


O.I 68 (Kdnig) 


0-88o(Kulish) 


0.510 (Stiassny) 


10 


0.085 


0-089 


0-162 


0-858 


0-528 


20 


0-100 


0-107 


0-163 


0-849 


0-550 


30 


0.123 


0-131 


O.I7O 


0-854 


0-574 


40 


0.154 


0.161 


0-183 


0.871 


O.6O2 


50 


0.193 


o . 198 


0-203 


0-902 


0-632 


60 


0.240 


0-243 


0-229 


0-946 


0-666 


70 


0.295 


0-288 


0-263 


1.003 


0.702 


80 


0-354 




0-300 


1.073 


0.742 


90 






0-347 


I.I57 


... 


100 


gms. H 2 


dissolve 0.193 g m 


n silver caproate, Ag C 5 H 


1A COO , at 50. 












(ruhner, 192/1 . ) 



SILVER CITRATE 

100 gms. H 2 dissolve 0.0277 gm. 



at 18, and 0.0284 gm. at 25. 

(Partheil and Hiibner, 1903.) 



SILVER Mitroso p PHENYL HYDROXYLAMINE . Ag [C fi H s .N(NO)03 . 

The solubility in water of the precipitated silver salt of nitrosp 
phenylhydroxylamine obtained by adding a solution of "cupfcrron"- (C fi H 5 .N 
(NO)b.NH 4 ), to a solution of a soluble silver salt, was determined at 
18 by potent iomefric and comluctometric methods. The results showerl 
i.4.io" 3 gm. atoms Atj per liter, equivalent to 0.150 gm. AR C 6 H fi N(NO)0 
(Pinkns and Martin, 1927.) 



Ag ARGENTUM 

SILVER BENZOATE 



24 



18.0 

20.0 
25.0 
25.0 



SOLUBILITY OF SILVBR BENZOATB IN WATER 

On. Mol. (tea. 

per liter per liter 



Authority 



1.763 (Holleman, 1893.) 

0.01038 2*375 (Larson and AdeL, 1931.) 

2.17 (Bphriam and Pfister, 1925.) 

0.01144 2.61 (Noyes and Schwartz, 1898.) 

0.01162 2.66 (Kolthoff and' Bosch, 1932.) 



op SILVER BRNZOATB AT 25 IN AQUBOTJS SOLUTIONS OFJ 
(Noyes and Schwartz, 1898.) 



Nitric Acid 
Gms. Mols. per Liter. Gms. per Liter. 



Chloracetic Acid 
Gms. Mols. per Liter. Gms. per Liter. 



O 


o 
o 
o 
o 


HN0 3 . 

.004435 
.00887 
.00892 
.01774 
.02674 


cofolg. 
0.01144 

0.01395 

0.01698 
0.01715 
0.02324 
0.03071 


HNO,. 

0.280 

0-559 
0.562 
1.118 
1.686 


CCMDAg. 
2.607 

3-195 
3.889 
3.926 

5.321 
7.031 


CH 2 
CICOOH. 

O 
0.00394 
0.00787 
0.01574 


COOAg. 
O.OII44 
0.01385 

o. 01612 

0.02093 


CH 2 
CICOOH. 

O 

0-37* 
0.744 

1.487 


C 8 H 3 
COOAs. 

2.607 
3.172 
3.691 
4.792 



One liter of cold alcohol dissolves 0.169 gm. CeHsCOOAg; one liter of boiling 
alcohol dissolves 0.465 gm. (Liebermann, 1902.) 



SOLUBILITY AT 18 OF SILVER BENZOATE IN AQUBOITS SOLUTIONS OK: 

(Urson and Adell, 19S1.) 



Sodium Nitrate 
Gta. Mols, jper liter 


Potassium Nitrate 
Oto. Mols. per liter 


Barium Nitrate 
Gkn. Mols.j>er liter 


Sodium 

dm. Mols, 


Acetate 
. per liter 


NaNOg 


Ag CeHgCOO 


* KNO?$ 


Ag C 6 H 5 COO x 


/B *< N0 3>2 ~ 


Ag C 6 H 5 COO " 


'MS CH 3 COO 


Ag C 6 H 5 COO ' 


o.o 


0.01038 


0.05 


0.01172 


0.0 


0.01038 


o.o 


O.OID38 


0.10 


0.01215 


O.10 


0.01221 


0.06 


0.0121/f 


0.0090 


0.01055 


0.30 


0.01351 


0.30 


0.01363 


0.08 


0.01235 


0.0496 


0.01396 


0.50 


0,O1422 


0.50 


O.OllUM 


0.125 


0.01306 


0.0992 


O.O13O3 


1 .00 


0.01523 


0.80 


0.01476 


0.160 


0.01323 


0.2974 


O.Ol6o8 


2.OO 


O.01624 


1 .00 


0.01507 


0.20 


0.01366 






3.OO 


O.Ol6lO 


2.0O 


0.01593 














3.00 


0.01576 











539 



FERRUM Fe 



FERROUS SULFITK 



EQUILIBRIUM IN THE. SYSTEM FERROUS OXIDE, SULFUR 
DIOXIDE AND WATER AT 15 AND AT 25. 

(Terres and Ruhl, 1934.) 

The determinations were made by the syirthetic method. The authors 
give a diagram in the present paper but the numerical results are pub- 
lished only in their report in Reihefte zu den Zei tschriften des Vereine 
deutscher Chemiker No. 8 193/1 - Verlag chemie Berlin W 35 Cornelius str 
3. Estimating from the small diagram the following approximate values 
were obtained. 

Results at 15 Results at 25 



Hoi, percent^ in sac, aol. 



' FeO 


^Z ' 


o5 

1.0 


0.3 1 
0.6 


2.0 


1.2 


2.5 


l.f 


2.4 


2.0 1 


2.2 


3-5 


2.3 
2.6 


5-0 
7.0 


3.0 


8.1 



Solid 



Hoi, percent ^n sat, aol. 
__ __ 



Solid 



FeS0 3 .5H 2 0(?) 
" 



+ FetHSO ) (?) 
Fe(HS0 3 ) 2 (?) 



' F0 


30 g ' 


0.5 


0.75 


1.0 
i-S 


1.3 
1.6 


1.9 


2.0 


1.5 


2.9 


1.25 


4.0 


1.5 
2.0 


5.9 
7.6 


2.3 


8.3 



FeSQ s .sH 2 
' 



" +Fe(HSO,U?) 
Fe(HS0 3 ) 2 (?) 



SO 



The mixtures separated into two liquid layers at concentrations of S0 2 
between 8.5 and 93 Mol. percent. 

IRON SULFATE (Ferrous) FeSO^HaO. 

SOLUBILITY OF FERROUS SULFATE IN WATER. (Fracnckd, 1907.) 





Gms. FeSO 4 




Gms. 


t. 


per TOO Solid Phase. 


t. r 


cSQi per 100 Solid Phase. 




Gms.H 2 0. 




Gms. H 2 O. 


0.172 


1.0156 Ice 


45.18 


44 . 3 2 FeSO4.yH^O 


0.566 


4.2852 


50.21 


48.60 


1.063 


8.7054 


52 


50 . 20 


-I.5II 


12.713 


54-03 


52.07 


-1.771 


14.511 


56.56 tr.i>t. 


54.58 " +FeSO v4 H 2 O 


I .82Eutec. 17'. 53 Ice-fFeS0 4 . 7 H a O 


60. 01 


54.95 FeSO 4 . 4 H a O 


O 


15.65 FeS0 4 . 7 H 2 


65 


55.59 unstable 


+ 10 


20.51 


70.04 


56.08 


15.25 


23.86 


64.8 tr.pt- 


FeS0 4 .4H 2 +FeS0 4 .H 2 O 


20.13 


26.56 


68.02 


52.31 FeS0 4 .H 2 


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 


d l6 .6 of sat. 


sol. = 1.219] 




(Greenish and Smith, 1903.) 



SOLUBILITY OF FERHOUS SULFATE IN WATER. 
(Agdo and Barkholt, 1926.) 



t". d of sat.^sol. 

i.o ...... 1.140 

9.6 ...... 1.178 

21.0....... i.a33 

25.0 ..... i.y.55 



Gms. Fe S0 4 .7 11^0 
per 100 gins. sal. sol. 

25. '25 
3r,32 
39.02 
4i.o8 



t" '/ of sat. sol. 

34.o ...... r.3ri 

43.o ..... 1.363 

54-0 ..... i.43s> 

80.0 ...... i.3(>7 



Gms. Fc SO, .7 H, 
per 100 gms. s;U. sol. 

48.65 
55'. 01 
63. 1 8 
55.49 



Fe 



SO 



FERRUM 54 o 

SOLUBILITY OP FBRRIC SULFATB IN AQUEOUS SOLUTIONS 

OF FSRROUS SULFATE AT 25 AND AT 50. 

(Cameron, 1936.) 

The mixtures were agitated for seven months. 
Results at 25 Results at 50 



Ona. per 


100 gns. 


sat. sol. Solid 


Qma. per 


100 ju. 


aat. sol. solid 


' FeSO f 


V 80 ^* 


V 


/ FeS0 4 I 




Excess^ Phase 
SO+ 


0.38 


44.75 


1.48 B.F.S. 


0*19 


48.73 


0.78 B.F.S. 


0.82 


44.15 


1.93 


0.67 


46.54 


2.59 


1.36 


43-79 


3.19 " 


3.67 


44.50 


1.33 " 


2.O1 


43-32 


2.98 " 


6.18 


41.03 


3.16 "tFeSO-.-; 


2.6l 


43-25 


1.12 " 


8.02 


38.87 


5.20 " 


3.07 


<|2.60 


1.56 " + FeSO A .7H !> 


10.55 


36.6l 


2.50 " " 


5-30 


38.42 


3.61 " 


14.74 


32.94 


1.09 FeSQ 4 .7fLO 


8.16 


36.60 


1.90 Fe 2 (S0 4 ) 3 + " 


19.40 


25.35 


..42 

0.95 


10.47 


28.36 


0.25 


21.76 


19.85 


1.01 " 


15-23 


16.64 


0.04 " 


27.88 


9.67 


0.22 " 


20.24 


5-73 


0.21 " 


30.35 


5.40 


O.30 " 


22.50 


1.36 


0.63 " 


31.99 


2.79 


0.67 



B.F.S.= Basic Ferric Sulfate* At concentrations of FeSO less than 
8.16 percent at 25 and 14.74 percent at 50 the nature of the solid 
phase is uncertain. 

SOLUBILITY OF FERROUS SULFATE IN AQUEOUS SOLUTIONS OF 
SULFURIC ACID AT VARIOUS TEMPERATURES. 



On. per 100 



Results at. o 



(Cameron, 1930.) 
a,,. ptr loo 



oi. 



Soll<1 



per 10Q 



1.8l 
4.10 
8-45 
15.56 
17.76 
25.98 
32.50 
36.05 
38.62 
41.80 
53.25 
6-3.60 



14.1 Fe7 

13-8 

11.10 " 

8.93 " 

7.67 " 
4.80 

399 " 

3-64 " 

,3-38 " 

2.34 Fei 
0.55 

0.28 " 



Fei 



Results at 25 



1.13 

3.41 

6.32 

^37 

13.00 

17.34 

24.54 



22.88 Fe7 

20.6l| " 

18.67 

16.79 " 

15.56 " 

13.25 " 

11.23 " 



Results at 25 Coi 


27.78 


10.70 


Fe 7 


31.00 


8.50 


Fei 


35-66 


5-89 


11 


41.47 


3.07 


" 


45*70 


1.75 


11 


54.71 


0.97 


11 


60.23 


0.56 


" 


64.35 


0.40 


11 


Results 


at 55 





1.74 


33.48 


Fe 7 


2.43 


32.76 


M 


3.87 


31.91 


" 


5-93 


29.20 


Fei 


7.73 


26.87 


M 


11.44 


24.34 


11 


22.26 


15.42 


11 


31.30 


9.25 


11 


45.37 


3.03 


II 


56.49 


1.01 





69.20 


0.61 


" 



Fei 



Results at 65 


i. 


82 


34 




24 


Fe/i 


i. 


61 


34 




66 


" 


3- 


29 


32 




57 


FC2 


10. 


21 


25 




11 


II 


16. 


32 


20 


. 


48 





29. 


4-6 


10 





38 


II 


Results at 


75 




0. 


43 


31 


t 


46 


Fe2 


3- 


45 


28 


. 


00 


11 


5- 


60 


25 


. 


58 


11 


8. 


71 


22 


. 


60 


M 


10. 


78 


21 


. 


29 


" 


21. 


90 


14 


. 


40 


" 


27. 


72 


11 


. 


26 


II 


34. 


72 


7 





05 


II 


Fe 7 


= 


FeS< 


1 


7H 


Q 


Fe4 - FeSO 


4 4 ^; 


? 'o 


Fe2 


= 


FeS< 


D 







Fei 


- FeSO 


!' 2 N ; 


8 o 



Tiie author also gives a review of the literature pertaining to the 
properties of ferrous sulfate, especially its solubility in presence of 
other salts. 



54i FERRUM 

SOLUBILITY OF FERRIC SULFATE AND OF FERROUS SULFATE IN Ao 
SOLUTIONS OF SULFURIC ACID AT 25. (Wirth, i9i 2 - I3 .) 



Fe 



Results for Ferric Sulfate. 



Results for Ferrous Sulfate. 



Normality of 
used Acid. 


Gms. per 100 Gms. Sat. 
Sol. 


Normality o 
used Acid. 


, Gms. per 100 Gms. Sat. 
lf Sol. 


Fe 2 3 * 


Fe 2 (S0 4 ) 3 . 


FCOOS SB 


FeSO,. 


2.2S 
6.685 


9.99 


25.O2 
14.58 


2.25 
IO.2 


10 
5-414 


19.03 
10.30 


19.84 


0.02 


0.05 


12.46 




7.26 








I 5- I 5 


2. II 


4.015 








19.84 


0.08 


o. 152: 



Solid Phase. 

FeS0 4 .7H 2 

u 

FeS(XH 2 



xi-- " ' * J " * 

EQUILIBRIUM IN THE SYSTEM FERRIC OXIDE, SULFURIC ACID AND WATER AT 25. 

(Cameron and Robinson, 1907.) 

^ (Excess of freshly precipitated ferric hydroxide was added to ferric sulfate solu- 
tions ot varying' conc* iir| *" | * s| '*" innc or "^ +v\** -.;<., -~~ *. ^.i^_ _t._i t . . \ 



Sat" Sol. 


Gms. per 100 Gms. 
Sat: Sol. 


Solid 
Phase. 


Gms. per 
Sat. 


' S <3 GmS - Solid 


Fe 2 3 . SO 3 . ' 


FeoO.,. 


*sor Phase - 


I 


.001 


o .07 





.11 Solid Solution 


20 


.48 


26 


1 8 F^Os ^SOg 


I 


.Oil 


O 


.62 





94 


Li 


19 


77 


28 


93 


I 


.045 


2 


03 


2 


65 


" 


10 


.87 


31 


35 Fe 2 O 3 .4S0 3 i 


I 


.131 


6 


.l8 


7 


.40 


(C 


O 


.16 


35 


.96 


I 


.217 


10, 


03 


ii , 


.84 


tl 


o 


.07 




.19 


I 


.440 


IS- 


,90 


20. 


.70 


(I 


I 


05 


42- 


43 



EQUILIBRIUM IN THE SYSTRM FERRIC OXIDE, SULPURIC ACID AND WATER. 

(Koenter ana Caiderwuod, 19:58.) 

Weighed samples were agitated in sealed glass bottles for various 
lengths of time and allowed to settle. The. liquid and solid were sepa- 
rated by filtration using a fritted glass filter. This required con- 
siderable time and the operation was conducted in the constant tempera- 
ture bath. Both the filtrates and the moist solids were analyzed. 
s. per 100 gfl. aat. sol. Sulla QMS. per 100 ja. sat. aol. 3oild 



Fe 23 


S0 3 v Phase ' 


F *23 


' *3 


' Phu, 


Results 


at 10 


Results 


at 15 


(con . ) 


2.76 


4.12 SS 


14.20 


28.25 


Fe .3$0 


7.32 


12.59 


17.11 


31.01* 


*" 3 i8H 2 8 


16.30 


25.88 


18.75 


31.94* 




2.23 

6.70 
o.o 


16. 191 Pe 0,+ 2./J4SO, 
31.27J * 8:6 5 H 2 3 
37.23 SS 


17.75 
10.30 

7.25 


31.85* 
30.90 
32.31 


Fe e 3 .4.6S0 3 


0.4 


45-00 " 


2.48 


35.23 


" 


0.27 


48.40 " 


0.80 


36.40 





0.41 


50-. 10 " 


O.O1 


37.20 





o.o/i 


74.50 " 


3.59 


30.60 


Fe 8 . 5 .8SO 


Results 


at 15 


0.77 
0.01 


3a.8o 
37.20 


;; . 3 oH 2 o? 3 






7.02 


29.39* 


t 


12.46 


16.60 SS 


0.98 


30.32* 


" 


14.61 


21.23 


13.18 


32.84 


Fe .3. 3^0 


15-70 


23.05 


10. 04 


33.21 


" . 10. 3H 


16.63 


24 . oo " 


2.48 


35-23 


" z 


17.61 


26.45 " 


0.80 


36.40 





16. 10 


25.40 Pe 2 3 .3SO i8H 


0.01 


9-33 


" 


15-86 


24 . 98 " 


14.09 


33.8o* 


" 


14.47 


26.15 


15.65 


42.27* 


" 



SO 



Supersaturated, SS = Solid Solution 



FERRQM 54^ 

EQUILIBRIUM IN THE SYSTEM FERRIC OXIDE, SULFURIC ACID AND WATER 

(Appleby and Wilkos, 1922.) 

Results at 18. Results at 25. 



Cms. per JIM) gins. 


sat. 


sol. 


Fe a 3 . 


S0 3 . 


0.21 


4o.64 


O.gi 


36.45 


6.48 


32.43 


8 . oo 


Hi. 85 


9 .63 


3i.88 


11.69 


3o.8o 


i3.88 


*9-7 


17.48 


29.73 


18.68 


29.64 


17.96 


*5.4ft 


14.00 


17.71 


1 1. 60 


i3.85 


6. 8 1 


7.60 



Solid Phase. 



H-f-Basle solid solut. 

Basic solid solutions 



Cms. per 


loo gras. 




sat. 


sol. 




^- ifc ^ 
F S 3 . 


*^ "* 
S0 3 . 


Solid Phase. 


0.27 


39-77 


Fe 2 3 .4S0 3 .9H 2 


0.71 


3 7 . * 





2.38 


34-99 





3.88 


33.20 


)) 


8.<>4 


32 . 06 


Fe 2 0;; . 3 S0;t . 7 H 2 O 


io.55 


30.77 





i3.8o 


3 0.02 


)> 


17.02 


29.86 , 


, 5(Fe 2 3 .3SO 3 ).2Fe 2 3 


i8.56 


29.98 





19-98 




Basic solid solutions 


19.78 


27 . 90 





iq.55 


25 .99 





i5.53 


1 7 . 62 


)> 


i3.5i 


14.58 





7-9' 


8.19 






EQUILIBRIUM IN THE SYSTEM FERRIC OXIDE, SULFURIC ACID AND WATER 
AT 50 TO 200. (Posnjak and Mcrwin, 1922.) 

gQ The authors give a critical discussion of previous work on this system. Their own 
determinations were made with the greatest possible accuracy. The identification 
of the solid phases was made both microscopically and analytically. Sealed tubes 
were used and at temperatures above 5o the tubes were heated by means of a 
resistance furnace within a steel bomb. The time required for equilibrium, varied 
from 2 months at 5o to only a week or 10 days at the higher temperatures. 

Results for the Isotherm at 50. 



Solid Phase. 



Fe 4 O a 



Fe,O 3 .4SO :) .3H 2 



Similar data for the 75, 1 10, 140 and 200 isotherms are given and also several 
determinations at i3o, i5o and 3oo. 

The following supplementary determinations upon this system at 50 
are given by Tunell and Posnjak, 1931. 



Gras. p^r 100 gms. 
sat. sol. - 


Cms. per 100 gins,* 
sat, sol. 


FegOj.- SO S . 


Solid Phase. 


^iF^oT^ 


S0 3 . 


O 


.14 


o 


.39 


Fe 2 3 .H,0 


20. 


70 


28. 


4o 





.3 9 


o 


79 





16. 


78 


3o. 


72 





.90 


i 


.53 





10. 


26 


3i . 




I 


.44 


2 


.3o 


))-4-3Fe s O s SQa.011,0 (?) 


8. 


56 


32. 


52 


2 


.55 


4 


.08 


3Fe 2 3 .4SO n .9H,0 


5. 


55 


33. 


96 


5 


.71 


9 


09 





0. 


34 


4i . 


18 


7 


-19 


ii 


19 





o. 


10 


48. 


44 


i5 


.43 


20 


.08 





o. 


()Q 


55. 


34 


16 


.09 


20 


.81 


)> 


o. 


07" 


59. 


20 


17 


.96 


22 


.96 


-t-Fe a 3 .2S0 3 .5lT a O 


o. 


08 


62. 


34 


20 




27 


.18 


Fe,0 3 .2SO 3 .5H 2 


o. 


07 


7 5. 


37 



>H-Fe 3 3 .:JSOj.7H a O 

.3S0 3 .7H 2 O 



Cto. per 100 pga. sat, aol. 



Solid 
Phase 



0.01 
1*95 



0.10 
2*94 
3.57 



99.89 
95-11 



aFe.CL.iiSO.^ILO 



543 FERRUM Fe 

EQUILIBRIUM IN THR SYSTEM PBRRIC OXIDB, SULFUR 
SULFUR TRIOXIDE AND WATER AT 25. 

(Baskervilie and Cameron, 1935.) 

Manv 'series of determinations were made upon mixtures prepared in 
different ways and agitated for various Lengths of time. For periods 
of as long as a year. The limiting members of the solid solutions ap- 
peared to be ferric oxide on the one hand and on the other a compound 



approaching the composition Fe 0, .2. sSO, 

<o O O 

d. o f Gms. per 100 Oms. per 100 
sat. gms. saj. sol. Solld gms. safc, sol. 


. 7 H 2 0. 

Oms. per 100 
Solld pa. s^: sol. SoUd 


sol. 


F 


B a3 


S0 3 


h'nase 


Fe ? 


3 


so 


3 


Phase rj~ e 


23 


so 3 ' ase 


1.052 


2 


45 


35S 


SS 


15 


ia 


29 


14 


l.2i.7 6 


.90 


32.06 1.4.9 


1.104 


4 


.86 


6.83 


II 


15 


.94 


28 


.88 


" 4 


.70 


32.68 " 


1.229 


9 


.86 


12.55 


II 


16 


.70 


28 


.00 


" 2 


03 


34.33 " 


1.242 


10 


19 


12.98 


11 


17 


31 


27 


45 





.26 


38.72 " 


1.328 


12 


33 


18.17 


" 


18 


.21 


26 


85 


" 


.03 


56.79 


397 


15 


52 


19.21 


11 


19 


.06 


26 


77 


8 


4 


31.8* " + 1.3.8 


500 


17 


.19 


23.96 


" 


16 


4 


28 


.2 


" tl-3-9 10 


34 


30.96 1.3.8 


471 


16 


67 


24.67 


II 


14 


49 


28 


.28 


1.3-9 8 


94 


31.54 " 


550 


19 


.08 


25.22 


It 


12 


.18 


28 


.88 


11 14 


7 


30.3* "+ 1.2.5.7 


590 


17 


95 


28.95 


fl 


11 


.06 


28 


92 


8 


. 11 


31.88 1.4.9 





20 


5 


26.4 


"+. 


9 


31 


29 


.64 


7 


.96 


31.86 










1.22 


.7 ? 


.2 


32 


.1 


"+1.4-9 






* Metastable 


i.2a 


7 


Fe 


P 3 .2. 


5 S0 3 . 7 H 2 0; 


1.3 


9 


= Fe 


2 3 . 3 S0 3 .9H 


2 0; i 


.4.9 = Fe 2 3 . 


4S0 3 ..9 


fl 2 


; i. 


3-8 = 


Fe 2 3 . 


3 so s 


.8H 2 


0; 


SS 


= Solid Solution 



EQUILIBRIUM IN THE 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 roo Gms. 

( Sat ^ Sol. So ii d Phase> Sat. Sol. golid Phase. 

Fe 2 O a . SO*. FeA. S0 3 . 

7 1 . 23 not det. 14 . 49 3 1 . 45 unstable 

0.24 56.84 " 15.71 31.88 

Sprob. Fe 2 (S04) 3 .H 2 SO 4 .9H 2 2O.2I 31.30 u 

+Fe 2 (S0 4 ) 3 .H 2 S0 4 . 3 H 2 
6.65 32.15 Feo(S0 4 ) 3 .H 2 S0 4 .8H 2 ^'^ 6 ' 54 

9-39 3 I -54 " -r-FeCsojj.HjSO^HjO ii. 06 29.43 

12.03 31.51 Fe(S0 4 ) 3 .H 2 S0 4 .8H : >O 13.88 28.33 

13.27 31.84 " 15.23 27.92 

13.68 31.78 unstable 16.07 27.98 

Results are also given for the two forms of yellow ferric sulfate (a copiapite and 
# copiapite) also for ferric hydroxide and sulfate solutions. 

It was found that a saturated solution of Fe^SO^a.HrjSO.i.SH/) in abs. alcohol 
at 25 contained 8 gms. Fe. 2 O 3 + 17.18 gms. S0 3 (Ratio, 1 14.235) per io<) gms. sat. 
sol. 

The yellow ferric sulfate Fe 2 (S04)3.9H20 .is less soluble in alcohol. After 4 
weeks snaking at 25, 100 gms. of the sat. solution in abs. alcohol contained 4.497 
gms. FeaOs and 6.779 S ms - ^-^ (Ratio, 1:3.006). Thus the alcoholic solution, 
just as the aqueous, is considerably more acid than the solid phase with which it 
is in equilibrium. 

IOO grams sat. solution in glycol contain 6 gins. FeSOa at ordinary temperature. 

(de Coninck.) 
IOO gms. anhydrous hydrazine dissolve I gm. ferrous sulfate at room temp. 

with decomposition. (Welsh and Brodeison, 1915.) 



so 



Fe FERRUM 



544 

, lw ^-^J T Lta for mixtures of ferrous sulfatc and 100 per cent stilfuric 
acid are given by Kendall and Davidson, 1921. 
FERRIC SULFATE 

SOLUBILITY OF FBRRIC SULFATF, IN AQUEOUS SOLUTIONS OF 
POTASSIUM SULFATB AT 25 AND VICB VERSA. 

(Cameron. 1936.) 

1. Solid 

"\ Phase 

1.2.1M- + K.SO. 



Ckus. pr 100 gg 


is. sac. sol. Solid 


Ores, per 100 gF 


^L.. 3 .^!..: 


/ K,S0 4 


Fe (SO ) k Phase 


K 2 S 4 


Fe ? (So 4 ). 


2.83 


27.8 1.2.14 


11.7 


0.85 


2.)4 


2<N3 


12.2 


1.25* 


3-34 


21.8 


12.5 


1-53* 


3.38 


20.8 


13-1 


1.68* 


4.56 


13.1 


13.7 


1.88* 


5-43 


11.2 " 


11.9 


0.6-) 


5-32 


9.02 " 


11.8 


0.31 


6.21 


6,04 " 


11.5 


0. 10 


8.0 


2. 35 " 


ii-3 


0.02 



* Probably points on a boundary curve of a four component system. 
1.2.14 = Fe 2 (S0 4 ) 3 .2K 2 S0 4 .i4fl 2 
The solutions contained a variable small excess of S0 4 



SO 



FERROUS Potassium SULFATE FeS0 4 .K 2 S0 4 .6H 2 0. 



SOLUBILITY IN WATER. (Tobicr, 1855.) 



f Gms. K 2 Fe(SO 4 )o 
1 per 100 Gms. H 2 0. 


t e . 


Cms. K 2 Fe(SO 4 ) A 
per 100 Cms. H 2 0. 


O 


19.6 


35 


41 


10 


24-5 


40 


45 


14-5 


29.1 


55 


56 


16 


30-9 


65 


57-3 


25 


36.5 


70 


64.2 



FERROUS Potassium SULFATE FeK 2 (S0 4 ) 2 .6H g O. 

SOLUBILITY OF MIXED CRYSTALS OF IRON POTASSIUM SULFATE 
AND ZINC POTASSIUM SULFATE IN WATER AT 6.8. (Habr-Chuwts, I92fi.) 
Gms. per 1000 cc. sat. sol. . Mol. per cent 



f .sat. sol. 


FftR s (SO,) s . ClI a O. 


ZnK s 7sOv).ir a O. 


in Solid Phase. 


. :>.o6" 


329.15 


0.00 


IOO.O 


. 1869 


275.03 


19^9 


<)3.55 


.175B 


246.80 


^8.8-2 


<)o.o8 


.1606 


.203 . :>'>- 


47 . 6-2 


8 1 .<)8 


.1474 


173.59 


53.07 


76.98 


. 1 339 


i4^7^> 


63.87 


69. 4S 


. 1204 


119.46 


67.83 


()4.29 


.io85 


87.69 


7*.* . 46 


.55.30 


.0795 


68.10 

v O.OO 


77 *-7* 
113.62 


47- aa 

. OO 



545 FERRUM 

SOLUBILITY OF FERROUS SULFATE IN Ao. SOLUTIONS OF LITHIUM SULFATE AT 30. 

AND VICE VERSA. (Schreinemakers, 1910.) 



Fe 



Cms, per IPO Gins. Sat. Sol 



' * 



24-87 
2 4-45 

2I -*5 
18.79 



^ 

FeS0 4 .7H 2 



1 6. 1 1 



o 
4 

5-58 " 

ii. 16 " 

15-81 

16.50 " +Li 2 S0 4 .H 2 O 

SOLUBILITY OP FERROUS SULFATB IN AQUEOUS SOLUTIONS OF MANGANESE 
SULFATE AND VICE VERSA. 



Cms, per 100 Cms. Sat. Sol. 
'"FeS0 4 . " Li2 SO, ' 

16.80 
18.31 
22.15 
23 iq 
25. 1 5 



15.39 

12.68 

5.32 

3.74 

o 



Li 2 S0 4 .H 2 



Results at o 



(White, 19?53.) 

Results at 25 



CJna. per 


100 gms. sac. aol. Solid 


fins, per 


100 eras. sat. sol. solid 


' MnS0 4 


FeS0 4 


s Phase 


' MnSo 4 


FeS0 4 ^ Phase 


3-07 


12.55 


Fe.7H E OSS 


0.09 


23.09 Fe. 7 H ? OSS 


5O3 


11. 44 




2.55 


21 .Ul " 


10.66 


9.26 





6.82 


18*94 " 


16.52 


6.84 


" 


10.33 


16.62 


19.18 


S.69 


" 


13.57 


14-39 " 


29.30 


1.25 


M 


24.96 


7.78, 


31.28 


0.34 


" 


36.95 


1.82 


31. 84 


0.14 


" 


37.83 


1.33 " * Mn.sH 








38.29 


0.85 Mn. 5 H 2 OSS 








39-39 


O.^ll 


Fe. 7 H 2 OSS = FeSO 
Penta hydrate Solid 


Hepta hydrate 
Solution. 


Solid Solution; Mn. 5 FLOSS ~ NnSO 

2 


FERRIC 


Ammonium SULFATE (Alum) (NII 4 ) FeJ S( 


^ 4 ) 4 24fl,0 



SO 



ioo cc. H 2 O dissolve .14.15 gms. anhydrous or 124.40 gms. hydrated salt at 
25 . Sp. gr. of saturated solution at 15 = 1.203. (Locke, 1901.) 



FERROUS Ammonium SULFATE (NHj Fe(S0 4 ) .6lf 
SOLUBILITY IN WATER. 

(Tobler; at 25, Locke Am. Ch. J. ZK.K., 459, '01.) 



I2 -5 25 2 5 .o(T) 50 4 o 

15 ^o.o 25 35-*(L) ?o 52 

40 33 .o 

SOLUBILITY OF AMMONIUM SULFATE IN AQUEOUS SOLUTIONS OF FERROUS 
SULFATE AT 30 AND VICE VERSA. 

(Schreinemakers, 1910 a.) 



Gms. per ioo Gms. 
Solution. 


Sat. 


Solid Phase. 


Gms. per ioo Gms. Sat. 
Solution. So ii d p hasft 


(NH,) 2 S0 4 . Kc.->u 4 : 




(NH 4 ) 2 S0 4 . 


FeSO,. 




44 


.27 


o 




(NHt) 2 S0 4 


8 


.90 


17 


.64 


1.1.6 


43 


.88 


o, 


79 


(NH)SO+i.i.6 


6 


-44 


23 


-59 


((. 


34> 


,24 


i . 


.72 


1. 1.6 


5- 


,91 


25- 


24 


i.i.6+FeS0 4 .7H 2 


19, 


.64 


5- 


.70 




5 


.24 


25- 


24 


FeS0 4 .7H 2 


16, 


.29 


7- 


95 


a 


o 




24. 


.90" 


u 



1.1.6 = (NH 4 ) 2 S04.FcS04.6H 4 0. 

Data for the quaternary system (NH 4 ) 2 S0 4 -f- FeS0 4 + Li 2 S0 4 + H 2 O at 30 
arc also given. 



Fe 



SO 



FERRUM 546 

IRON Ammonium SULFATE (Ferrous) Fe (NH 4 )j (SO 4 )->.6H 2 0. 

SOLUBILITY OF MIXED CRYSTALS OF IRON AMMONIUM SULFATE 
AND ZINC AMMONIUM SULFATE IN WATER. (Gstersetzer, 1926.) 

The two salts mix in all proportions. The influence of temperature upon the 
solubility is insignificant, in that the relation between the solubilities of the two 
salts does not change with increase of temperature. 



Results at 7. 

Gras. per jooocc. sat. sol. 


Wt. per cent 


Results at 8. 5. 

Gms. pc i* JflOOcc. sat. sol. 


\Vl. P<T C'Hll 




' ^^ 


s^**- , 


FciNII,) s (SO,) s 


-- "mi 


^ ^**~ 


FelNHtMSO*} 


c. of 


Fo(NH,)i 


Zn (Nil,), 


.GH 2 in tl of 


Fc{NH,)a 


Zn O'HJ, 


.611,0 in 


at. sol. 


.(SO,) 2 .KH 2 0. 


.{S0 4 ),.GII,0. 


Solid Phase. sat. sol. 


.(SOt),.GH,0. 


.(S0 4 ) 2 .r,H s O. 


Solid Phase. 


:i54i 


279.49 


O.OO 


ioo. o 1.1578 


286.52 


O.OO 


1 OO . O 


.1454 


236.84 


18.99 


85.17 


.1452 


243.71 


24.00 


87.12 


.139-2 


220. 2 4 


22.47 


76.07 


.1366 


212.66 


34.99 


71.40 


.1877 


181.49 


4o . i o 


59-99 


.i3t>4 


i83.i3 


45.93 


:")6.76 


. 1203 


i58.6o 


46.88 


49-52 


.1184 


J57.54 


54.60 


49-5f 


.ui5 


125.20 


62.89 


3 7 . 7 4 


.1121 


i33. 7 o 


63.35 


38.4-2 


. io5i 


ioi.64 


70.93 


29.51 


. io35 


103.70 


72.90 


27.46 


.0965 


73.58 


82.46 


18.19 


.0963 


78.82 


81.59 


i8.63 


. 09 1 2 


54.36 


92. lo 


i3.i8 


.0891 


53.45 


95.04 


11.56 


0794 


o.oo 


125.00 


o.oo 


.0873 


27.65 


112. 25 


5. 7 8 










.0798 


o.oo 


i28.3o 


. 00 



FERRIC SULFATE 

SOLUBILITY OP FBRRIC SULPATB IN AQUEOUS SOLUTIONS 
OF AMMONIUM SCLPATE AT 25. 

(Cameron. 1936.) 
Oms. per 100 gms. sat. sol. Solid Gtos. per 100 gms. sat. sol. Solid 



(NH 4 ) 2 S0 4 


Fe 2 (S0 4 ) 


s Phase 


1.4 


44.5 


? 


1-5 


44.2 


? 


1.7 


44.4 


1.1.24 t ? 


1.9 


43.1 


1.1.24 


2.2 


39-2 


ii 


3-3 


32.8 


n 


4.8 


28.7 


" 



(NH 4 ) 2 S0 4 


Fe 2 (S0 4 ), 


5 v Phase 


11.7 


20.6 


1 . 1 . 24 


14-8 


18.0 


" 


17.3 
26.6 


16.3 

9.0 


11 + (NH 4 ) 2 S0 4 
(NH 4 ) 2 S0 4 


40.8 


1.4 


11 


44.2 


0-5 


11 



1.1.24 = Pe 2 (S0 

The Solutions contain 



4 ) 3 .(NH 4 ) 2 S0 4 .24ligO 
ontained a variable 



small excess of SO 



V 



FERROUS SULFATE 

SOLUBILITY OP FERROUS SULFATE IN AQUEOUS SOLUTIONS 
SODIUM SULPATE.AT 97 AND VICE VERSA. 
(Benrath and Benrath, 1929.) 



OAS. per 100 gms. 

-A. 


sat. sol 


Solid 


Qms. per 100 gms. 


sat* sol 


Solid 


Na 2 S0 4 


FeS0 4 


^ Phase 


Na 2 S0 4 


FeS0 4 


s Phase 


0.0 


19-57 


FeS0 4 .H g O 


23.30 


6.68 


1.1.2 


1.92 


18.47 


11 


24.91 


6.51 


" t 1,3 


5.69 


16.12 


" 


25-99 


4.93 


1.3 


14.15 


11.50 


11 


27.17 


3.94 


" 


16.60 


10.48 


11 


28.81 


2.32 


" 


19.22 


11.20 


" + 1.1.2 


28.11 


2.35 


II . M j 


19.72 


10.33 


1.1.2 


29.09 


1.46 


Na 2 S0 4 2 ' 


22.87 


7.32 


n 


30.50 


0.0 


fi 4 



1.1.2 = FeS0 4 .Na 2 S0 4 .2H e O; 1.3 r FeSO A . 3 Na 2 S0 4 



547 GALLIUM 

SOLUBILITY OF MIXTURES OF FERROUS SULPHATE FeSO 4 .7H 2 O AND 
SODIUM SULPHATE Na 2 SO 4 .ioH 2 O IN WATER. 

(Koppel Z. physik. Chcm. 52, 405, '05.) 



Ga 



Gms. per 100 Gms. 


Gms. per TOO Gms. 


t. Solution. 


H 2 O. 




FeSO 4 . 


Na 2 SO 4 . 


'FeSO 4 . 


Na 2 SO 4 . 


O 


14-54 


4-93 


18.06 


6. ii 


IS-5 


17.76 


11.32 


25-05 


T 5-97 


21.8 


16.57 


I5-32 


24-34 


22.51 


24.92 


16.21 




23.62 


22 .04 


35 


l6 -35 


14.98 


23.91 


21.83 


40 


16.37 


15.42 


24.01 


22 .62 


.18.8 


18.13 


13-8 


26.63 


2O.28 


23 


19.58 


12.5 


28.82 


18.4 


27 


20.97' 


"3 


3-95 


16.64 


31 


22 .91 


9.71 


33-99 


14.41 


35 


23 .85 


9.26 


35-66 


13-85 


40 


26.32 


7-85 




II .92 


18.8 


18.23 


14.83 


27.23 


22.16 


23 


13^3 


18.04 


20.31 


26.48 


28 


7-66 


24.41 


11.28 


35-94 


3 1 


4-58 


29.50 


6-95 


44-75 


35 


4.04 


3 -49 


6.16 


46.58 


40 


4.10 


30.60 


6.27 


46.99 



Solid Phase. 



FeSO 4 .7H 2 + N 



FeNa 2 (SO 4 ) 2 .4H 2 O 



.icH 2 O 



GALLIUM HYDROXIDE GaiOH) s . 

SOLUBILITY OK (JTALLIUM HYDROXIDE IN AQUEOUS SOLUTIONS 
OF SODIUM HYDROXIDE AT 18-20. f Fricke and Hlom-ku, littS. ) 



OH 



Nonnulih 


Cuts. GH,O.. t 


of aq. NnOM. 


por ion cc. snl. s'l. 


I .^9 


0.77 


3.65 


2.01 


7.^7 


4.24 


9.61 


7.01 


io.34 


q.o-2 


10.37 


8.H3 



.\onuuCt\ 
of aq. M.-iOII. 

I I .01 



1-2.6S 

iS.'ati 

i5.37 



7.1-2 

5.98 



a-94 

2. -2B 



GALLIUM SELENATE Ga,( 

An excess of air dried gallium solcnatc was add<nl to wat(r an<l the mixture 
kept at '25 for 6 hours. Constant shaking is not mentioned. Samples of the 
clear supernatant solution were weighed and I heir content of gallium determined 
by the sodium sulfitc method. 

100 gms. of the saturated solution contained rj..o5 gms. (/a 2 3 at v.5. 

( Dennis and JJricl-mjm. 1018. 



GALLIUM Ammonium SULFATE (Alum) GaNH 4 (S0 4 ) g i2H 2 0. 

ion re. sal. solution in water contain .To. 84 gins. NrJ^Ga(SO i ). i! . r; HL (.) at '.>:)". 

)> f>(>"/ a I ro IN > I o. <>i?i 7 J > 

i) 70/ (l 0.00875 

a' niixl. oi'iJj ec. of II, -} So cc. of C..,II : ,OH -- |5 n-.. rone. H^SO^ 

contain o.i6i3gms. NH^ (la ( SO A ).,. rp.ILO at ~l$. "(Do.nnis and Bridgman, HUB.) 



SO 



Gd GADOLINIUM 54* 



GADOLINIUM BROMATE Gd(BrO_),.c 

O O 



SOLUBILITY OP GADOLINIUM BRCfcATB IN WATBR. 

(Janes, Fogg, Mcjntlre, Evans and Donovan, 1927.) 



t o 


0ms. Od(Br0 3 ) 3 .9H 2 


Solid 


r o 


Qms. Od(Br0 3 ) 3 .9H 2 Solid 




per 100 8fna. HgO 


Phase 


L 


per 100 pis. H g O Phase 





50.18 Gdl 


IBrO ) . 9 H C 


> 25 


110.5 GdtBrO,), 


5 


6o.0l 


it 


30 


126.1 


10 


70.11 


M 


35 


144-5 


15 


82. 6i| 





40 


166.0 


20 


95. 5^ 


it 


45 


195.6 



GADOLINIUM ACETATE Gd(GH : >GOO) 3 .4H. 2 O. 

100 gms. sat. sol. .of gadolinium acetate in water contain 10.87 g m - G<* (CH 3 C00) 8 
at 25. ( Meyer and Mrtller, 1*0. I 

GADOLINIUM LACTATE. Gd(G 3 H 5 O 3 ) 3 .i 1 / 2 H 2 O. 

.100 gms. sat. sol. of gadolinium lactate in water contain o.i54 gms. Gd 2 : j, 
equivalent to 3.833 gms. Gd (C 3 H 6 3 ) a .i 1/2 H a O, at 20. ( Jantsdi, me. i 



GADOLINIUM GLYCOLATE Gd 2 (C 2 H 3 O 3 )3.2H2O. 

IOOO CC. H 2 O dissolve 14.147 gms, of the salt at 2O. (Jantsch and GrUnkraut, 1912-13.) 

CH 

GADOLINIUM SULFONATES. 

SOLUBILITY IN WATER. Gms 

Salt. Fonnula. *"- Authorit y- 



Gms. H 2 O. 

Gadolinium m Nitro- I nArmi SKrr\\cr\i TT r\ Q f (Holmberg, 

benzene Sulfonate J Gd[aH 4 (NQ B )SO.],.7HaO 15 43-8 5 



Gadolinium Bromoni- [ r-jrr-rr T> /xr^\^r\ / \T T T ^ * $ (Katz and 

trobenzene Sulfonate ^d[C 6 H 3 Br(NO 2 }oO 3 (i.4.2)l3.ioH 2 O 25 6.31 



GADOLINIUM CobaltiCYANIDE Gd 2 (CoC 6 N 6 ) 2 .9H 2 O. 

IOOO gms. aq. 10% hydrochloric acid dissolve 1.86 gms. of the salt at 25. 

Games and Willard, 1916.) 

G4DOLIHIOM OXALA.TE Gd g (C 2 4 3 .ioH 2 

SOLUBILITY OF GADOLINIUM OXALATE IN AQUEOUS 20% SOLUTIONS OF 
^ Uu METHYLAMINE OXALATE, ETHYLAMINE OXALATE AND TRIETHYLAMINE OXALATE. 

(.Grant and James, 1917.) 

Solvent. Gms - G d2(CA) 3 per 

100 cc. Solvent. 

Aq. 20% Methylamine Oxalate 0.069 

" Ethylamine " 0.360 

Triethylamine " 0.883 



549 GADOLINIUM 

SOLUBILITY OP GADOLINIUM OXALATB IN AQUEOUS SOLUTIONS OR ACIDS' AT 25. 

(Sarver and Brlnton, 1927.) 

The determinations were made gravimetrically by evaporating large 
volumes of the saturated solution. 



Gd 



Solvent concentration 
in normality 

0.1008 iiCl 

0.2576 " 

O.SOOq. " 
1.018 

1.484 " 
2. 



Oms. 

100 e 



sat. sol. 



Solvent concentration 
In normality 



* o.i (COOH), 



0.5 



* sat. 



0.0024 
0.0099 
O.0329 
0.0938 
0.1563 
0.2457 
0.006l 
0.0525 

o. 1448 

0.3777 
0.0011 
0.0037 
0.021< 
0.0676 
0.0026 
0.0475 
0.1921 



UNO, 



0.5 (COOH), 



II j. 



sat. 



.000 

0.978 

2.000 
2.865 
3.965 
0.978 
2.OOO 
2.865 
3.965 

4-0 

6.0 

GADOLINIUM OXALATE Gd 2 (C 2 04) 3 .ioH 2 0. 
SOLUBILITY IN AQUEOUS SOLUTIONS OF SULFURIC ACID AT 25. 

Solid Phase. 



1.992 

4.054 

2.0 

3.03 

4.00 

2.0 

3.03 

4.0 

4.0 

6.0 

o.oe* " 2 S0 4 
0.419 " 
0.958 " 
1.846 " 
2.612 " 



Oms. ilrd^fCrtO.) per 
tOO gms. sat. sol. 



o.i 



(GOGH) 



Normality of 
Aq. HUSO,. 

2.16 

3-n 

4-32 
6.I7S 



Cms. per TOO Gms. Sat. Sol. 



0.2785 
0.9032 
0.0768 
. 28 i 3 

0.54.98 
0.0128 
0.0'|63 
0.1397 
0.0383 
0,1227 
0.0086 
0.0401 
0.0988 
0.2047 
0.2970 



(Wirth, 1912-) 



GdsOa. Gd 2 (C'A) 3 . 

0.1883 o -35 

0.3010 0.4803 " 

0.4359 0.6956 " 
0.707 1.128 " 

GADOLINIUM Magnesium NITRATE, etc. 

SOLUBILITY OF DOUBLE NITRATES OF GADOLINIUM AND OTHER METALS IN CONC. 
NITRIC ACID OF dy = 1.325 ( = 51.59 GM. HN0 3 PER 100 cc.) at 16. (Jantsch,i9i2.) 

Gms. Hydra ted 

Salt. Formula. Salt per Liter 

Sat. Solution. 

Gadolinium Magnesium Nitrate [GdCNC^ekMgs^HkO 352.3 

Nickel " " Ni 3 " 400.8 

Cobalt " " Co 3 " 451-4 

Zinc " " Zn 3 " 472.7 

GADOLINIUM Dimethyl PHOSPHATE Gd 2 [(CH 3 )2PO 4 ]6. 

100 gins. II 2 O dissolve 23 gms. Gd 2 [(CH 3 )2P0 4 ]6 at 25 and 6.7 gms. at 95. 

(Morgan and James, 1914-) 

SOLUBILITY OP GADOLINIUM DIMETHYL PHOSPHATE IN WATER. 
(Marsh, 1939.) 



100 



Gtas. Od ? 3 per 
I leer sac. aol. 



O 37.0 126 

25 2^.2 82.3 

SO l$.7 S3- 4 

The saturated solution at o was prepared by mechanical stirring 
for 3-4 hours. For the other temperature* the cold saturated solution 
was diluted somewhat and stirred occasionally for 3-4 hours. 



coo 



NO 



PO 



Gd GADOLINIUM 55<> 

GADOLINIUM SULFATE Gd 2 (SO 4 ) 3 .8H 2 O. 

SOLUBILITY IN WATER. (Benedicks, 1900.) 

t ^ Cms. Gc^S^per ioo Solid Phase. 

o 3 .'98 * Gd2(SO 4 )3.8H 2 O 

10 3-3 

14 2.8 

2'5 2. 4 

34.4 2.26 " 

100 gms. H 2 dissolve 2.886 gms. Gd z (S0 4 ) 3 .8H g O at 20 and 2.19 gms. 
at 40^. (Jackson and Pienacker, 1930.) 



SOLUBILITY OF GADOLINIUM SULFATE IN AQUEOUS SOLUTIONS OF: 

Sodium Sulfate at 25. (Bissell and James, 1916.) Sulf uric Acid at 25. (Wirth, 1912., 

^r^Q^GdTsO^ S ' UdPhase - oPigsoF Gm Gd P Q ' Gd' SO*' ^ S Ud Phase ' 

so o 4< 2. K i5 43 " Gd 2 (S0 4 )3.8H 2 O o 1.793 2^1' G<MS0 4 )s.8H 2 

u 0.43 2.06 " o.i 1.98 3.291 " 

0.47 0.76 Gd2(SO4)3.Na2SO4.2H2O 0.505 2.365 3.931 " 

1.26 0.17 " i.r 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 " 



GERM4NIUM Tetra CHLORIDE GeCl 4 

MISCIBILITY OP GERMANIUM TRTRA CHLORIDB AKD SULFUR DIOXIDE. 

(Bond and Crone, 1934.) 

The synthetic method was used and the temperatures of melting or 
disappearance of the second liquid layer determined. 

Oma. 0C1 per 



(ftl 

100 e 


i. oeci 4 per 
pis. SAC., sol. 


uni 

C 100 ( 


i. (jeui pr 

zjns. sac. sol. 


r<> 

C 100 8 


gms. sat. 


5i.8(m.pt.) 


100. 


-4.9 


63.98 


-51.5 


7.0 


75.0^-53.9 ) 


1 98.80 


-4.9 


63.06 


-55.2 


6.26 


6i*.9(-55*,o] 


1 97-97 




59.87 


-6o.5(-58.o) 


5-15 


53.0 
46.6 
31.0 
27.2 
24.2 


97.97 
96.4! 
93-72 
92.72 
91.76 


-4.7 
-4.9 
-5.1 

-5-5 

-6.2 


58.81 
52.37 
49.92 
45-00 
41.86 


-73.o(-64.5> 
-76.11-66.8) 
-79.21-66.8) 
-86.o(-7i.8) 


4.21 

3.48 
3.07 
2.71 

2.17 


21.1 


90.58 


-7.4 


37.78 


-88.o(-72.8) 


2.07 


"15.0 
"12,3 


87.42 
85.54 


-9.0 
-10.1 


34-22 
31.95 


(-76.5) 
1-76.5) 


1.55 

1.48 


-9.2 


82.24 


-13.1 


27.52 


(-76.1) 


0.94 




78.62 


-24.6 


17.52 


(-75-9) 


0.72 


-all 


75.36 


-32.7 


13.16 


(-75.5) 


0.00 


-5.2 


69.42 


-36.4 


11.31 






-5.2 


68.78 


-41.2 


10.07 






-5.0 


67.59 











The figures in parentheses are melting points. 



551 GERMANIUM Ge 

SOLITBILITY OP GERMANIUM DOUBLK FLUORIDES IN WATER, EACH 
DETERMINED SEPARATELY. 

(Mtiller. 1927.) 



German liun 
Double Fluoride of: 


Kormula 
of Salt 




Oms. 


Salt per 


tOO^cc sat. 


solution at,: 




' 


10 


25 


70 


40 


ec 


lithium 


GeLi ? F 6 








53.92 











Sodium 


GeNa F 


1.52 


1.68 




2.25 


2.8 3 


3.36 


Pot ass i urn 


fJ<ak P k 1 

vjcri\ r*. 


0.25 


0.363 


0.59 




0.95 




Rubi di u.m 


GeRb-F fl 


0.23 


0.302 




0.74 








Caesium 
Tell urium 


GeCcF e 
GeTeV 




0.98 


1.89 


2.28 
34.58 








Silver 


GeAg ? F 








_ 


88.03 









GERMANIUM DIOXIDE Ge0 2 . 

loo gms. H 2 O dissolve 0.405 gm. Ge0 2 at 20, and 1.07 gms. at 100. (Winklcr, 1887.) 



SOLOBILITY OP GERMANIUM DIOXIDE IN WATER. 

(Schwarx and Huf, 1931.) 

The Germanium dioxide was prepared by distilling germanite 4-5 times 
in a stream of chlorine, freeing the tetrachloride tMis obtained of 
chlorine by means of Hg and hydrolysing in distilled water. Several 
determinations made with such samples gave the following results at 20, 

Preliminary Hours allowed Ona. (X0 g per 

treataent of aaaple for saturation 100 cc'aat. sol. 

Hydrolysis 6 hrs. with 30.6% H 2 30 0.534 

" with 3.7* H g O drying 

over KOH 14 hrs, age 58 hrs. 35 0.596 

Hydrolysis of Ge0 2 , heated 2 hrs. at 600 28-51 0.430 

" " " " " " " MO o 143 0.349 

Boiling in H 2 (hydrolysed, dried) 0.74? 

Melted GeO ? 32 0.572 

The following results at different temperatures were obtained with a 
preparation which had been heated to 600 and was used in the ratio of 
0.4 gm. per 100 cc H 2 0. 

t 11 20 ?6 36 41 

Gms. Ge0 2 per 100 cc sat. sol. 0.396 0.430 0.470 0.551 0.617 

A table of results is also given showing that the variations of 
solubility of Ge0 2 in Water depends upon the preliminary treatment of 
the sample as well as upon the ratio of solid to water used in the de- 
termination. 

The properti es of themodif ications of GeO obtained by various means 
are described by Miiller and Blank, 1924; and Miiller, 1926. 



Ge GERMANIUM 



GERMANIUM DIOXIDE 



552 







SOLUBILITY OP GERMANIUM DIOXIDE IN AQUEOUS SOLUTIONS 
OF HYDROCHLORIC ACID, SULPURIC ACID AND SODIUM HYDROXIDE AT 25. 

(Pugh, 1929.) 

The object of the determinations was to obtain evidence of the ampho- 
teric character of germanium hydroxide and supply comparative values of 
the acid and basic dissociation constants of this compound. The GeO g 
was prepared from the pure disulfide by repeated treatment with UNO. 
and ignition to bright red heat. The oxide, which had not been allowed 
to fuse, was ground with water, washed until free of H g S0 4 and finally 
reignited. It was found that 8-10 days agitation were necessary for 
attainment of equilibrium. 



Results for 


Results for 


Results for 


aq. Hydrochloric Acid 


aq. Sulfuric Acid 


aq. Sodium Hydroxide 


0m. Mols. HC1 Oms. OeO ? per 


Qm. Mols. H 2 S0 4 Oms. OeOg per 


Om. Mols. per liter sat. sol. 


per liter lOOcc sat. sol. 


per liter loocc sat. sol. 


' NaOH Oeo 2 > 


o.o 0.4470 


o.o 0.4470 


o.o 0.0428 


0.25 0.4H5 


0.50 0.3550 


0.00125 0*0440 


0.50 0.3810 


0.98 0.2805 


0.0025 0.0483 


1.50 0.2600 


l.<0 0.2000 


0.005 0.0545 


2.0 0.21&5 


2.05 0.1600 


o.oio 0.0675 


2.925 0.1544 


2.52 0.1305 


0.0125 0.0746 


3.85 0.1140 


3.02 0.099 


0.025 0.1115 


4-35 0.0920 


3-50 0.074 


0.050 0.1693 


5.20 0.074 


4.0 0.050 


o.ioo 0.2280 


5.72 0.102 


4.5 0.041 




6.23 0.1820 


5.85 0.019 




6.85 0.3164 


795 0.009 




7.62 0.7660 


(95$> 0.140. 





Fusion-point data for mixtures of GeOj, + K g O and GeO p 
given by Schwarz and Ileinrich, 1932. 



NaO are 



GERMANIUM (Mono) SULFIDE GeS 
GERMANIUM (Di) SULFIDE GeSa. 
loo gms. HaO dissolve 0.24 gm. GeS 
loo gins. HoO dissolve 0.45 gm. GeS 2 . 



(Winkler, 1887.) 



100 ?ms. liquid NII 3 dissolve 0.0473 gm. GeS (= 0.0031 Gm. Mol. GeS 
per liter) at -33. 

100 gms. liquid NH dissolve 3.112 gm. GeS g (= 0.1551 Gm. Mol. GeS 2 

a*l'*>A.tn+_. _0 /T^.U____ 1 tTI ^.1 _ i 



per liter) at -32. 9 



(Johnson and Wieatley, 1934.) 



553 HYDROGEN H 

HYDROGEN H,. 

SOLUBILITY OF HYDROGEN IN WATER. 
(Milligan, 1924.) 

Hydrogen mixed with air was shaken for i minutes with distilled water previously 
saturated with air. The gas phase was analyzed by means of a Haldarie gas analysis 
apparatus before and after contact with the water and the amount of hydrogen 
dissolved was estimated by difference. It was found that i cc. of H 2 at 26 dis- 
solves 0.017 cc. hydrogen (reduced to o) when the pressure of the gas over the 
water is 760 mm. 



SOLUBILITY OP HYDROGEN IN WATBR. 

(Winkler Ber. 24, 99, '9* 5 Boo* and Bock Wied. Ann. 44, 318, '91; Timofejew 2. pbysik. 

Chem. 6, 147, '90-) 






0.0214 


. . . 


. . . 


0.0214 


0.000193 


5 


0.0203 


0.0209 


0.0241 


0.0204 


0.000184 


10 


0.0193 


0.0204 


0.0229 


0.0195 


0-000176 


15 


0.0185 


O.O2OO 


0.0217 


0.0188 


0-000169 


20 


0.0178 


0.0196 


0.0205 


0.0182 


0-000162 


2 S 


0.0171 


0.0193 


0.0191 


0.0175 


0.000156 


3 


0.0163 






0.0170 


0.000147 


40 


0.0153 


. . . 




0,0164 


0.000139 


So 


5.0141 


. . . 




0.0161 


0.000129 


60 


0.0129 






0.0160 


0.000119 


80 


0.0085 


. . 




0.0160 


0.000079 


100 


O-OOOO 






0.0160 


o oooooo 



ft- Bunsen Absorption Coefficient which is the volume of gas (reduced 
to o and 760 mm) absorbed by i volume of the liquid when the pressure 
of the gas itself without the tension of the liquid amounts to 760 mm. 

ft~ Solubility, or the volume of gas (reduced to o and 760 mm) which 
is absorbed by i volume of the liquid at barometric pressure of 760 mm. 

y - the weight of gas in grams dissolved by 100 gms. of pure solvent, 
at the indicated temperature and a total pressure (that is, the partial 
pressure of the gas plus the vapor pressure of the liquid at the absorp- 
tion temperature) of 760 mm. 

I = the Ostwald Solubility Expression which represents the ratio of 
the volume (v) of gas absorbed at any pressure and temperature, to the 
volume (V) of the absorbing liquid, thus I - L This expression differs 
from the Bunsen Absorption coefficient ft in tnat the volume (v) of the 
dissolved gas is not reduced to o & 760 mm. The solubility / is there- 
fore the volume of gas dissolved by unit volume of the solvent at the 
temperature of the experiment. The two expressions are related thus: 

j 

I -ft( i+o. 003671), A- (1+0.003671) 



H 



I HYDROGEK 

HYDROGEN 



554 



SOLUBILITY OP HYDROGEN IN WATER AT VARIOUS TERMPERATURKS AND AT 
25 TO 1000 ATMOSPHERES PRES5URE. 

(Wiebe and Gaddy, 1934.) 

The authors used the same method previously employed at 25. The hy- 
drogen contained o.i percent N for which a correction proportional to 
its mol fraction was applied. A correction for change of vapor pressure 
due to the gas pressure on the liquid, was made. By a sensitive method 
of plotting deviations the experimental data were smoothed with respect 
to both pressure and temperature to obtain the following interpolated 
solubility values. 



Pressure In 
Atmospheres 

25 

50 
75 

100 

ISO 

200 
300 

400 

500 
600 

700 

800 

900 

1000 

Pressure in 
Atmospheres 



cc Hg (reduced to o and 760mm]^ dissolved by i.p On. Hj>0 at: 



7 


10" 


20* 


30" 


40" 


f^ 


0.5363 


0.4870 


0.4498 


0.4263 


Q.4133 


0.4067 


1.068 


0.9690 


0.8945 


0.8475 


0.8215 


0.8090 


1.601 


1-453 


1.341 


1.271 


1.232 


1.212 


2.130 


1.932 


1.785 


1.689 


1.638 


1.6l2 


3.168 


2.872 


2,649 


2.508 


2.432 


2*395 


4.187 


3.796 


3-499 


3.311 


3.210 


3.165 


6.139 


5.579 


5.158 


4.897 


4.747 


4.695 


8,009 


7-300 


6.766 


6.430 


6.245 


6.166 


9.838 


8.980 


8.328 


7.922 


7.705 


7.613 


11.626 


10.610 


9.856 


9.390 


9.135 


9.017 


13.370 


12.214 


11.362 


10.818 


10.524 


10.389 


15.013 


13.746 


12.808 


12.218 


11.889 


11.735 


16.548 


15.215 


14-.217 


13.583 


13-230 


13.072 


18.001 


16.623 


15.592 


14 928 


14-569 


14.404 



cc Hg (reduced to o and 760mm) dissolved by i.o 8m. HgO at: 



60" 


70 


80 


90 


10CP 


0*4053 


0.4093 


0.4203 


0.4385 


0.4615 


0.8O95 


0.8171 


0.8385 


0.8720 


0.9120 


1.211 


1.224 


1.254 


1.298 


1.355 


1.610 


1.628 


1.667 


1.727 


1.805 


2.393 


2 . 422 


2.485 


2.576 


2.681 


3.168 


3.208 


3.286 


3-402 


3.544 


4.692 


4.746 


4.866 


5.042 


5.220 


6. 173 


6.249 


6.392 


6.600 


6.841 


7.625 


7.717 


7.885 


8.129 


8.429 


9.0i6 


9.131 


9.324 


9.665 


9.994 


10.405 


10.527 


10.757 


11.093 


11 .512 


11.746 


11.893 


12.169 


12.555 


12.980 


13-084 


13.233 


13.533 


13.946 


14.394 


14.407 


14.557 


14.867 


15.303 


15.775 



25 

50 

75 

100 

150 

200 
300 
400 
500 
600 
700 
800 
900 
1000 

The authors extrapolated the results at 25 atmospheres to lower 
pressures by means of Henry's law to obtain values at one atmosphere. 
These results when converted to terms of the Bunsen and Ostwald coef- 
ficients agree fairly well with the data of Winkler except at the higher 
temperatures. 



555 HYDROGEN. H 

HYDROGEN H g 

SOLUBILITY op HYDROGEN IK WATER AT 25 AND AT 25 TO 1000 
ATMOSPHERES PRESSURE. 

(Wiebe, Gaddy and Helns, Jr., 1932.) 

The authors used a simple bubbling-type of apparatus made of a steel 
cylinder with pressure valves. Equilibrium Was approached from both 
lower and higher pressures. The experimental accuracy was about 0.5 
percent except at the lower pressures. 

Atsoospheres cc.Hg (reduced to o aiid-760auu) Atmospheres cc H g (reduced to and 760m) 

Pressure dissolved by i.o o. HgO Pressure dissolved by l.o &"- HgO 

25 0,<|.36 1 0.008 400 6.57 t 0.0'4 

50 0.86? 0.012 600 9.58 1 0.05 

100 1.728 t 0.017 800 12.46 1 0.06 

200 3.39 1 0.03 1000 15-20 1 O.o8 

Additional data for the solubility of H in water at pressures up to 
10 atmospheres are given by Cassuto, 1913. 

H 



SOLUBILITY OF HYDROGEN IN WATER AT 25 AND AT PRESSURES 
UP TO 150 ATMOSPHERES. 

(Frollch, Touch, Hogan and Peer, 1931.) 

The determinations were made by shaking water and hydrogen at various 
pressures in a steel cylinder maintained at 25, and, after attainment 
of equilibrium, withdrawing a sample of the mixture over mercury in one 
of three burets so designed that the volumes could be measured with the 
same degree of accuracy at any ratio of gas to liquid. The results are 
given in the form of a diagram from which the following approximate 
values were read. 

Pressure In cc. H^ (measured at 25 and 1 Atw. pressure) 

atmospheres dissolved by l.o cc HJO 

50 2.0 

80 3.0 

120 4.5 

ISO 5-5 



H HYDROGEN 556 

SOLUBILITY OP HYDROGEN IN WATER AT HIGH PRESSURES. 

(Ipatlew, Jr., Crush lma,-Artemowltsch and Tlchorolrow, 1931, 193?.) 

Mixtures of water and hydrogen under pressure were rotated in a steel 
cylinder at constant temperatures. Equilibrium was reached in compara- 
tively short periods of time. Samples of the mixture were removed to a 
buret containing mercury and the volumes of liquid and gas accurately 
measured at room temperature and the gas volume reduced to o and 76omm. 

H g Pressure In CC.H 2 (reduced to o A 760 w) CC. H^ (reduced to and 760wn) 
1 Atmosphere* dissolved in 100 cc H ? t dissolved In 100 cc H^Q at 100 

Atmospheres Pressure 

25 20 

40 

60 

80 

" 100 

" 120 

" 140 

100.0 ISB. 

In a subsequent paper by Ipatiew, Jr., and Theodorawtch, 1934, results 
for the Solubility of Hydrogen in Water at temperatures up to 225 and at 
pressures varying between 30 and 100 atmospheres, are given. 



SOLUBILITY OP A MIXTURE op 76.42 PERCENT HYDROGBK AND 25.58 PIRCENT 
NITROGEN IN WATER AT 25 AND AT 50 TO 1000 ATMOSPHERES PRESSURE. 

(Wleb and Oaddy. 1935.) 

The approximately 3.1 mixture of hydrogen and nitrogen was prepared by 
burning hydrogen in air. The amount of argon introduces an uncertainty 
of about 0.2 percent. The same bubbling method was used as previously 
employed by the authors for determinations of the solubility of hydrogen 
in water at different temperatures and pressures. The composition of 
the gas in the two phases was analyzed by means of a modified form of 
thermal conductivity apparatus containing glass instead of the usual 
metal cells, 



33-0 


0.5 


196.3 


66.4 


5-0 


188.0 


100.2 


10.0 


180.0 


132.8 


15.0 


174-3 


165.3 


20.0 


168.3 


199.2 


25.0 


165.5 


231.0 


35-0 


162.5 




45-0 


158.7 





cc H 2 ( reduced to 


Av. percent H g In the 


Av. percent H g In the 


Pressure in 


and 76Qnn) dissolved 


gas present In 


gas present in 


atmospheres 


In 1.0 9. HgO 


the liquid phase 


the gas phase 


50 


0.8349 


80. 17 


76.42 


100 


1.643 


80.89 


76.42 


200 


3-209 


82.68 


76.42 


400 


6.068 


84.33 


76.42 


GOO 


8.809 


84.92 


76.42 


800 


11.327 


85.32 


76.42 


1000 


13.724 


8S-8l 


76.42 



Thermodynamical calculations of the solubility of Hydrogen and Nitrogen 
and their mixtures in Water at pressures up to 1000 atmospheres based 
upon the above results are given by Krichevsky and Kasarnovsky , 1935, 
1936, and by Kielland, 1936. 



557 HYDROGEN 

SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF ACIDS AND 

BASES AT 25. 

(Geffcken Z. physik. Chem. 49, 268, '04.) 



Gram Equiv. 
AddsTsind 


Solubility of E 


I (fa "= Ostwald Expression) in Solutions of: 


Bases 
per Liter. 




HC1. 


HNO 3 . 


*H 2 S0 4 . CH 3 COOH. 


CH 2 C1COOH. KOH. 


NaOH. 


0-0 





.0193 





.0193 





.0193 





.0193 


0.0193 


0.0193 


0.0193 


0.5 





.0186 





.0188 





.0185 


O 


.0192 


0-0189 


0.0167 


0.0165 


1.0 





.0179 


O 


.0183 


P 


.0177 





.0191 


0-0186 


0.0142 


0.0139 


2.0 





.0168 





.0174 





.0163 





.0188 


0-0180 


... 


O.OO97 


3.0 


o 


.0159 





.0167 





.0150 


o 


.0186 




. . . 


0.0072 


4-0 






O 


Ol6o 


O 


.0141 


o 


.0186 






0.0055 



The above figures for the concentrations of acids and bases were calculated to 
grams per liter, and these values with the corresponding l^ values for the solubility 
of hydrogen , plotted on cross-section paper. From the resulting curves, the follow- 
ing table was read : 



Grams Acids 


Solubility of H (/2s = Ostwald Expression) in Solutions of: 


per Liter. HC1. HNO 8 . H 


[aSO*. CH 3 COOH. CH 2 C1COOH. KOH. 


NaOH. 








.0193 


0.0193 





.0193 





.0193 


0-0193 


0.0193 


O 


.0193 


20 





.0185 


0-0189 


o 


-Ol86 





.0192 


0-0191 


0.0172 


O 


.0165 


40 


o 


.0179 


0-0186 





.Ol8o 


O 


.0191 


0.0190 


0.0153 


O 


.0140 


60 





0173 


0-0183 





.0174 





.0190 


0.0188 


0.0135 


O 


.0117 


80 





.0167 


0-0180 . 


o 


.0168 


o 


.0189 


0-0187 




O 


.0097 


100 


o 


.0160 


0.0179 


o 


.0162 


o 


.0189 


0-0185 




O 


.0082 


150 






0.0171 





.0143 





.0188 


0-0182 







.0058 


20O 




. . . 


0.0165 





.0140 





.0186 


0-0179 








250 






0.0160 









.0184 




... 




... 



THE SOLUBILITY OF HYDROGEN IN CONC. H 2 SO4 AT 20. 

(Christoff, 1906.) 

%H 2 S0 4 o 35.82 61.62 95.6 

feo 0.0208 0.00954 0.00708 0.01097 

SOLUBILITY OF HYDROGEN IN AQUEOUS PROPIONIC ACID SOLUTIONS. 

(Braun, 1900.) 



Cms. QHsCOOH 
per 100 Cms. 
Solution. 

2.63 

3-37 
5-27 
6.50 
9.91 


Coefficient of Absorption of Hydrogen at: 


O.O2245 
O.O222 
O.O224 

0.0218 

O.O2I3 


10. 

O.O2I4 
O.O2I2 
O.O2I2 

o . 0209 
o . 0203 


rs- 
O.O2OO 
O.OI99 
0.0198 
0.0193 
O.OI9I 


20. 
0.0188 
O.OI87 
0.0184 
0.0183 
0.0178 


25. 
O.OI72 
O.OI7I 
O.OI7I 

.>.oi69 
0.0160 



SOLUBILITY OF HYDROGEN IN AQUEOUS SODIUM HYDROXIDE AND OTHBR 
SOLVENTS AT 100 ATMOSPHERES PRESSURE. 

(Ipatlew, jr., Drushlma-Artemowltsch and Tlchonlrrow, 1931-1938.) 

cc Hg (reduced to and 

t Solvent ?eo) Pr 100 cc solvent 

25 Ag. 20% NaOH Solution 41.7 

25 Methyl alcohol 869.5 

25 Benzene 694.11 



H 



H HYDROGEN 55 

SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OP AMMONIUM 

NITRATE AT 20. 

(Knopp~Z. physik. Chem. 48, 103, '04-) 



Normality Molecular 
4 (per 1000 Gms.) Conccntra- 
F HsO. tion. 


Absorption 
Coefficient 
of Hydrogen. 


Density 
of Solutions. 


O-OO 


o.oo 


o.oo 


0.0188 




1.017 


0.1308 


0.002352 


0.01872 


1.0027 


vJ / 

2.167 


0.2765 


0.004956 


0.01845 


I -0072 


3.378 


0.4363 


0.007799 


0-01823 


I.OI22 


/ o / 

4.823 


0.6333 


0-011280 


0.01773 


I .Ol82 


6-773 
"550 


0.9069 

1.6308 


0.016447 
0.028525 


0.01744 
0.01647 


1.0262 
1.04652 



SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF 

CHLORIDE. 

(Braun 2. physik. Chem. 33. 73St '<*>) 



BARIUM 



Gms.BaC3 2 


Coefficient of Absorption of Hydrogen at : 

^ . ..A . ...!. 


per 100 Gms. 
Solution. 


5. 


10. 


I5- 


20. 


25. 


o.oo 


0.0237 


0.0221 


O.O2O6 


O.OI9I 


0.0175 


3- 2 9 


0-02II 


0-0198 


0.0l85 


0.0172 


0.0157 


3-6 


O.O2O9 


0.0197 


0.0184 


O.OI7O 


0.0156 


6-45 


0.0196 


0.0186 


0.0173 


0.0161 


0.0147 


7.00 


O.OI94 


0.0183 


0.0172 


0.0159 


0.0146 



SOLUBILITY OP HYDROGEN IN AQUEOUS SOLUTIONS OF CALCIUM CHLOR- 
IDE, MAGNESIUM SULPHATE, AND LITHIUM CHLORIDE AT 15. 

(Gordon Z. physik. Chem. 18, 14, '95.) 

Coefficient of Absorption of hydrogen in water at 15 = 0.01883. 



In Calcium 


In Magnesium 


In 


Lithium 


Chloride. 




Sulphate. 


Chloride. 


Gins. 
CaCl 2 


G.M. 
CaCl 2 


Absorption 
Coefficient 


Gms. 
MgS0 4 


G.M. 
MgSO 4 


Absorption 
Coefficient 


Gms. 
LiCl 


G.M. 
LiCI 


Absorption 
Coefficient 


per 
xoo g. Sol. 


per 
Liter. 


of H. 


per 
100 g. Sol. 


per 
Liter. 


of H. 


per 
loo g. Sol. 


iSer. 


of H. 


3-47 


0.321 


0.01619 


4-97 


0-433 


0.01501 


3-48 


0-835 


0.01619 


6.10 


0-57S 


0.01450 


10.19 


0.936 


0.01159 


7-34 


I.SOO 


0.01370 


"33 


I. 122 


0.01138 


23.76 


2.501 


0.00499 


14.63 


3-734 


0.0099 


17-52 


1.1827 


0.00839 














26 34 


2.02 


0.00519 















.For definition of Coefficient of Absorption, see page 553 



SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF POTASSIUM 
CARBONATE, CHLORIDE, AND NITRATE AT 15. 

(Gordon.) 

Jn Potassium In Potassium In Potassium 
Carbonate. Chloride. Nitrate. 


(ims. 
KoCOs 

per 
100 g. Sol. 

2.82 
8.83 
16.47 
24.13 
4r.8r 


G.M. 

per 
Liter. 

0.209 
0.690 
I-376 
2. 156 

4-352 


Absorption 
Coefficient 
of H. 

0.01628 
0.01183 
0.00761 
0.00462 
O.00r6o 


Gma. 
KC1 
per 
100 g. Sol. 

3^3 
7.48 
12.13 

22.92 


G. M. 

KC1 
per 

Liter. 

0.526 
1.051 

1-755 
2.909 

3-554 


Absorption 
Coefficient 
of H. 

0.01667 
0.01489 
0.01279 
O.OIOI2 
0.0089? 


Gms. 
KNO 3 
per 
100 g. Sol. 

4-73 

8.44 
16 -59 
21.46 


G. M. 
KN0 3 

per 
Liter. 

0.482 
0.879 
1.820 
2.430 


Absorption 
Coefficient 
of H. 

0.01683 

0.01559 
0.01311 
O.OllSo 



559 

SOLUBILITY OP HYDROGEN IN AQUEOUS SOLUTIONS 
CHLORIDE AND NITRATE AT 20. 

(Knopp Z. physik. Chem. 48, 103, '04.) 



OF 



HYDROGEN 
POTASSIUM 



In Potassium Chloride. 


In Potassium Nitrate. 




p. 


Normality 
(per looo 
g. H 2 0). 


Absorption 
Coefficient. 


Density 
of 
Solutions. 




P; 


Normality 
(per rooo 
g.HjO). 


Absorption 
Coefficient. 


Density 
of 
Solutions. 


i 


.089 


0.1475 


0.01823 


I .0052 


I 


.224 


0.1245 


0.01835 


1.0059 


2 


.123 


o . 2907 


0.01757 


I .Oll8 


2 


.094 


0-2II4 


o. 01818 


I.OII3 


4 


.070 


0.5687 


o- 01661 


I .0243 


4 


.010 


0.4127 


0-01785 


I -0236 


6 


375 


0.9127 


O.OI53I 


1.0394 


5 


925 


0.6225 


0.01743 


1 -0359 


7 


.380 


I .0682 


0.01472 


I .0460 


7 


.742 


0.8293 


0-01667 


1.0477 


'3 


.612 


2.1222 


0.01255 


1.0875 


13 


.510 


I-5436 


0.01436 


1.0865 



SOLUBILITY OP HYDROGEN IN AQUEOUS SOPIUM CARBONATE AND 

SULPHATE SOLUTIONS AT 15. 

(Gordon.) 



In Sodium Carbonate. 



In Sodium Sulphate. 



Gms.Na 2 COs G.M. 


Absorption 


Gms. Na 2 SO 4 


0. M. 


Absorption 


per too Gms. Na 2 CO 3 


Coefficient 


per 100 Gms. 


Na 2 S0 4 


Coefficient 


Solution. per Liter. 


of H. 


Solution. 


per Liter. 


of H. 


2.15 0.207 


0.01639 


4.58 


0-335 


O.OI5I9 


8.64 0.438 


0.01385 


8.42 


0.638 


0.0154 


11.53 1.218 


0.00839 


16.69 


1.364 


0.00775 



SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF SODIUM 

CHLORIDE. 

(Braun; Gordon.) 



Gms.NaCl 


Coefficient of Absorption of Hydrogen at: 


Solution 


' 5. 


10. 


15. 


20. 


25. 


i -S 


0.0218 


0.02O5 


O.OI9I 


0.0177 


0.0162 


3.80 


0.0198 


0.0188 


0.0176 


O.OI62 


0.0148 


4.48 


0-0192 


0.0182 


O.Oiyi 


0.0159 


0.0143 


6.00 


0.0184 


0.0175 


O.Ol64 


0.0153 


0.0138 


14.78 






0-0093 






23.84 






0.00595 







SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF SODIUM 

NITRATE. 



In Sodium Nitrate at 20. 

(Knopp.) 



In Sodium Nitrate at 15. 

(Gordon.) 



f 


Normality 


Absorption 


Density 


Gms.NaNOs 


C. M. 


Absorption 


p> 


(per looo 


Coefficient 


of 


per too Gms. 


NaNOa 


Coefficient 




Gms. H 2 O). 


of H. 


Solutions. 


Solution. 


per Liter. 


of H. 


1.041 


0.1236 


0.01839 


I .0052 


5-57 


0.679 


0.01603 


2.192 


0.2634 


0.01774 


I.OI30 


II .16 


I-4I3 


0.0137 


4-405 


0.5416 


0.01694 


I .0282 


19.77 


2.656 


O.OIO52 


6.702 


0.8442 


0-01518 


I .04411 


37-43 


5-7II 


O.OO578 


12.637 


'7354 


0.0130 


1.08667 









H HYDROGEN 560 

SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF VARIOUS SALTS AT 15. 

(Steiner, 1894.) 
c u- A Bunsen Absorption Coefficient ft (Xio 4 ) in Aq. Solution oC Normality. 

stoft. T 7. I ^ ^~7. ^ G. ^ J? 

LiCl 1883 1574 1325 ii2i 949 

KNOa 1883 1524 1276 1076 

iAICk 1883 1511 1221 993 Sio 667 550 

KC1 1883 1502 1217 996 820 

NaNOa 1883 1496 1201 984 808 667 542 

iCaC! 2 1883 1493 1195 958 780 635 510 

NaCl 1883 1478 1144 38o 699 573 

jMgS0 4 1883 1451 1120 856 659 499 

1883 1446 1113 852 667 510 

1883 1370 991 710 

1883 1338 967 700 508 372 273 206 158 

1883 1340 699 

Cane Sugar 1883 1280 731 

SOLUBILITY OF HYDROGEN IN ALCOHOL. (Timofeicw, 1890; Bunscn-Heunch, is<j2.) 

Coef. of Absorp- Coef. of Absorp- Coef. of Absorption 

t. tionino8.8% t*. tioniny% t. in Pure Alcohol 

Alcohol. Alcohol . ( B u nsen ) . 

o 0.0676 4 0.0749 i 0.06916 

6.2 0.0693 18.8 0.0740 5 0.06847 

13.4 0.0705 11.4 0.06765 

23.7 0.06633 
SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 20 AND 760 MM. PRESSURE. 

(Lubarsch, 1889.) 
Wt. % Alcohol. Vol. % Absorbed H. Wt. % Alcohol. Vol. % Absorbed H. 

o 1.93 28.57 I -4 

9-09 i-43 33-33 i-i7 

16.67 1.29 50 2. 02 

23.08 I.I7 66.67 2.55 

SOLUBILITY OF HYDROGEN IN AQ. SOLUTIONS OF CHLORAL HYDRATE. 

(Mtitler, C 1912-13.) 





Cms. Chloral 


Absorption Coefficient. 




Hydrate per 




j^ 




t*. 


100 Gms. Aq. 
Sol. 


Solution. 


ft- 


fto- 


19.4 


15-5 


I .O722 


0.01732 


O.OI724 


17-4 


28.3 


I.I43 


0.01569 


O.OI54O 


18.7 


46.56 


1-2505 


0.01388 


0.01375 


16.5 


52 


I .2870 


O.OI3I4 


O.OI28O 


17 


63 


I-37I 


O.OI27O 


0.01243 


17.9 


68 


1.4097 


0.01286 


O.OI27O 


18.3 


78.4 


1-4993 


0.01398 


0.01380 


SOLUBILITY 


OF HYDROGEN IN 


CHLORAL HYDRATE SOLUTIONS AT 


2O. (Knopp, 1904.) 


P. 


Normality (per 
1000 Gms. H a O) 


Molecular 
Concentration. 


Absorption 
Coefficient of H. 


Density 
of Solutions. 


4.91 


0.310 


0-005594 


0.01839 


I.O2O2 


7.69 


0.504 


0.008992 


0.01802 


I.O32O 


14-56 


1.030 


O.OI8223 


O.OI7I2 


1.0669 


29.50 


2.530 


0.043601 


0.01542 


I . 1466 


3M2 


3-770 


0.063647 


0.01440 


I .1982 


49-79 


6 


0.0974Q3 


0-01353 


1.2724 


63.90 


10.700 


o. 161660 


0.01307 


1-3743 



For definition of Bunsen Absorption Coef., see p. 5 53 



56i HYDROGEN 

SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF GLYCEROL. 

Results at 14 and 21. (Henkel, 1905, 1912-) Results at 25. (Drucker and Moles, 1910.) 



t-. 


Wt. % 
Glycerol. 


Absorp. Coef. 
(See p. 227.) 


Wt. % 
Glycerol. 


rf H Sat. Sol. 


la (Ostwalcl 
Expression) . 


14 





0.0193 





I 


0.0196 


it 


2.29 


0.0189 


4 


I .OIOI 


0.0186 


(C 


5-32 


0.0186 


10.5 


1.0260 


0.0178 


(C 


8.57 


O.OI82 


22 


1.0542 


0.0154 


tt 


10.83 


O.Ol8l5 


49-8 


1.1290 


0.0099 


tl 


15.31 


0.01765 


50.5 


1.1300 


0.0097 


21 


O 


0.0184 


52.6 


1.1365 


o . 0090 


n 


2.29 


O.OlSl 


67 


1.1752 


0.0067 


" 


5-68 


O.OI77 


80 


1.2113 


0.0051 


a 


6.46 


0.0176 


82 


1.2159 


0.0051 


n 


10.40 


O.OI7I 


88 


1.2307 


0.0044 


tt 


18.20 


0.0160 


95 


1.2502 


0.0034 



Additional data for this system are given by Miiller, C. 1912-13. 
SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF SEVERAL COMPOUNDS. 

(Htifner, 1906-07.) 
Cone, of 

Solvent Gms. t. Absorption Cocf. 0. 

per Liter. 

O 2O. II O.OlSl 
41.45 20 0.0176 

87.3 20.25 0.0166 

174 20.28 0.0152 

60 20.17 0.0170 

59 20. ii 0.0180 



Aqueous Solution of: 

Water alone 

Dextrose (Grape Sugar) 



Urea 

Acetamide 

Alanine 

Glycocol 



89 

75 



0.0156 
0.0158 



SOLUBILITY OF HYDROGEN IN AQUEOUS SOLUTIONS OF CANE SUGAR AND 
OF GRAPE SUGAR. (Mailer, c. 1912-13.) 



Wt. ' 



15.2 
ii. 6 
12 

12.7 
ii. 8 

J 3*3 
12.6 



5- 
14. 

20. 
29. 
31- 

42. 


04 

7 
26 
86 
74 

94 


di* 

4i 
d u 
d\s 

dw 
d\* 


.5 = 

5 = 


I 
I 
I 

I 
I 

I 


.OI9 
.060 
.084 
.128 
.133 

-195 



wt. % 

Grape 
Sugar. 



Sp. Gr. 
Sat. Sol. 



Abs. Cocf. 



19.3 

20.5 

20 

21 

21 

21 



Q 
12.2 ^20=1.048 

20.7 <f2o=io84 
32.56 ^20=1.130 

"1 = 1.199 
1=1.266 



45.8 
59 



0.0184 

0.0160 
0.0145 
0.0125 

O.OIO2 
0.0078 



(Goidon, 1895.) 



Abs. Coef. 
ft*. 

0.0173 
O.OI5I 
0.0146 
O.OI26 
O.OII9 
O.OIO3 
O.OO94 

SOLUBILITY OF HYDROGEN IN AQUEOUS SUGAR SOLUTIONS AT 15' 

Gms. Sugar per Gm. Mols. Sugar Absorption 

roo Gms. Solution. per Liter. Coefficient of H. 

16.67 0.520 0.01561 

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. Gelatin , 
per 100 cc '"'" 

1.53 0.0194 

2.6q 0.0189 
4.74 0.0185 
5.71 0.0182 



Dextrin. 
Gms. Dextrin Sn r , r , 


Starch. 
Gms. Starch Sn rr 


/., 5 . 


pen 


[00 CC. 










per 


roo cc. 










3 


.98 


I 


.OI2 


O 


.0194 


2 


.OI 


I 


.005 


O 


.0194 


8 


.58 


I 


.OIQ 


O 


.OIQI 


3 


-56 


I 


.Oil 


o 


.0189 


8 


.12 


I 


.028 


o 


.0188 


7 


13 


I 


.024 


0.0181 


19 


.20 


I 


.066 





.0174 


9 


.29 


I 


.032 





.0182 



HYDROGEN 562 

COMPARATIVE SOLUBILITY OF HYPROGIN AT 38 AND ATMOSPHBRIC 
PRBSSUKS in WATER AMD IN Ox BLOOD SERUM AND CELLS. 

(Van Slyke and Sendroyjr., 1928.) 
floltrent Abs. Cof. cc H g pr l cc sat. sol. 

Water 0.01630 

Aq. 0.15 normal NaCl 0.01559 

Ox Blood Serum 0.01533 

Ox Blood Cells o. 



SOLUBILITY OF HYDROGEN IN WATER AND IN RUBBER. \ 

(Vcnable and Fuwa, 1922.) ff 

The gas dissolved by a given amount of air free rubber was pumped out with I 

a TOpler pump and measured over mercury. | 

100 cc. HjO dissolve 1.8 cc. hydrogen (reduced to o and 7,6o mm ) at 21. 
Rubber less than i.occ. ( ) 

RATIO OF THE SOLUBILITY OF HYDROGEN IN WATER TO ITS SOLUBILITY 

IN AQUEOUS SOLUTIONS OF SUCROSE AT 15. 

(Garner and Masson, 1921.) 

Mols. sucrose per liter 0.292 O.585 0.877 1.169 i f .46o 1.755 

Ratio, H a in H 2 H 2 in aq. sucrose, i.ii 1.23 1.39 1.61* i'.87 2.17 

SOLUBILITY OF A MIXTURE OF 3 VOLUMES OF HYDROGEN + I VOLUME OF NITROGEN 

IN LIQUID AMMONIA. ( Larson and Black, 1925. } f, 

Cc. Gas (at standard U'lnp-ancl pressure) 
dissolved by 1 .0 gin. liquid Ammonia 



Tolal Pressure. t- 

5o atmospheres 25.2 


II,. 

I 62 < 


N,. 
>.73 


Total. 
2.35 




18 5 


I GO < 


).84 


2.74 






'> 07 < 


>.o4 


3.01 




3 o 


2 35 


.08 


3.43 






2 6 1 




3.76 




)> _|- 2 5 


> Ht\ 




3.89 






3. IQ 


16 


4.65 




100 atmospheres 25. o 


3 30 


.35 


4.65 




20. o 


3 (56 


46 


5.12 




16.5 


3.85 


.63 


5.48 


i, 




/, 43 


83 


6 . 26 


t 


5.2 


4.84 


i 02 


6.86 


l> 




5 28 i 


t 28 


7.56 


t 


-4-22 o 


7 54 ^ 


J.2I 


1 . 75 




i5o atmospheres 22.0 


4.70 


.89 


6.59 




1 7 2 


5 . 1 2 t< 


> O(t 


7.21 




Q o 


6 . 20 t< 


i.44 


8.64 








*.58 


8.88 




... . -h 5 O 


8 22 


5 33 


n.55 




i3.3 


0.42 


).6i 


i3.o3 





HYDROGEN II 



563 

SOLUBILITY op HYDROGEN IN LIQUID AMMONIA AT SEVERAL 
TEMPERATURES AND AT PRESSURES up TO 1000 ATMOSPHERES. 

(wiebc and Tremearne, 1934; Wlebe and Oaddy, 193?.) 

The steel tube bubbling apparatus previously described for the 
solubility of II in Water was used. The K g contained 0.1% N ? and the 
NH g contained 0.02% H p O. No correction was made for these impurities. 
The values are believed to be accurate to within 2-3 parts per 1000. 

Total Pressure 
Itv Atmospheres 

25 

50 

75 
100 
150 
200 
300 
400 
500 
600 
700 
800 
900 
1000 

Ipatjew, and Theodorowitch, 1932, give results for the solubility of 
Hg in liquid NH^ at 25 and at pressures up to 250 atmospheres which are 
somewhat lower than the above over their whole range. , 



cc Hg (reduced to o and TOOmm^dlssolved by i.o gn>. 


NH 3 at: 


' 


85 


50 


75 


100 ' 


' 


1.695 


0.85 








3.28 


4-47 


5-10 


3-49 








7.20 


9-33 


9-95 


5.80 


6.70 


9.88 


13-49 


16.35 


15.67 





15.08 


21.60 


29 00 


36.35 


13.11 


20.08 


29-39 


41.41 


57.10 


18.96 


29.45 


44.42 


65.40 


98.74 


2M.33 


38.13 


58.33 


88.34 


140.60 


29.27 


46.18 


71.33 


110.22 


182.4 


33-99 


53.71 


83.^8 


131 .0 


224.0 


38.25 


60.77 


94.82 


150.6 


264.3 


42.33 


67.63 


105.4 


169.2 


305.2 


46.20 


73-7-4 


115-3 


186.8 


3^6.5 


49.77 


79.25 


124.9 


203.3 


388.. 2 



SOLUBILITY OF HYDROGEN IN RUSSIAN PETROLEUM. 

(Gnicwasx and Walfisz, 1887.) 

Coefficient of absorption at 20 = 0.0582, at 10 = 0.0652. 



SOLUBILITY 
Results in terms 


OF 

of 


HYDROGEN IN WATER AND IN ORGANIC 
the Ostwald Expression, 


SOLVENTS. 

(Just, 1901.) 


Solvent. 




fe. 




A-o- 


Solvent. 




k. 


/JO- 


Water 


o. 


,0199 


0. 


0200 


Amyl Acetate 


o. 


,0774 


0.0743 


Aniline 


o. 


0285 


o. 


0303 


Xylene 


o. 


.0819 


0.0783 


Amyl Alcohol 


o 


.0301 


o. 


0353 


Ethyl Acetate 


o, 


.0852 


0.0788 


Nitrobenzene 


o 


.0371 


o. 


0353 


Toluene 


o. 


,0874 


0.0838 


Carbon Bisulfide 


o 


0375 


o, 


0336 


Ethyl Alcohol (98.8%) 


o, 


, 0804 


0.0862 


Acetic Acid 


o 


0633 


o. 


.0617 


Methyl Alcohol 


o. 


0945 


0.0902 


Benzene 


o 


.0756 


o, 


,0707 


Isobutyl Alcohol 


0.0976 


0.0929 


Acetone 


o 


.0764 


o 


.0703 











SOLUBILITY OF HYDROGEN IN ETHYL ETHER. 

(Christoff, 1912.) 

Results in terms of the Ostwald Solubility Expression / 

/o = 0.1115, /5 = 0.1150, /io = 0.1195, /,5 - 0.1259. 



II HYDROGEN 



Results for the system, Hydrogen + Nitrogen -f Ammonia (gas) + Ammonia 
(Liquid) at temperatures from -22.5* to +18.7' and pressures from 50 to 
1000 atmospheres are given by Larson and Black, 1925- A discussion of 
these and similar results for other systems in light of the concept that 
solubility effect is a change in activity of one component resulting 
from the presence of the other component is given by Cupples, 1929. 



H 



HYDROGEN 

SOLOHILITY OF HYDROGEN IN SBVBRAL SOLVENTS. 
(Horiuti, 1S31.) 

The determinations were made with great precision. The results are 
in terms of the Ostwald Solubility Expression, which is I = the ratio 
of the concentration of the hydrogen in the liquid phase to its con- 
centration in the gas phase. 

Results for: 



art) on 


Tetrachloride 


Benzene 


Ethyl Ether 


t 


i 


t 


I 


t 


I . 





0.0650 


7.0 


0.0585 


-80.6 


0.0498 


20.9 


0.0794 


22.9 


0.0700 


-59-9 


0.0632 


38.8 


O.0928 


41.3 


0.0844 


-40.0 


0.0800 


59.0 


. 1 1 24 


62.8 


0.1051 


-21.1 


0.0964 










0.0 


. 1 188 










21. 1 


0.1409 




Acetone 


Chlorobenzene 


Methyl 


Acetate 


t 


l 


t 


i 


c 


t 


-81.9 


0.0273 


"40.9 


0.0303 


-78.5 


0.0249 


60.7 


0.0376 


-20.5 


0.0382 


-60.3 


0.0338 


40.6 


0.0498 


0.0 


0.0479 


-40.1 


0.0447 


20.9 


0.0618 


21 .2 


0.0595 


-20. 1 


0.0578 


0.0 


0.0783 


40.0 


0.0702 


0.0 


0.0730 


20.9 


0.0968 


60.3 


0.0837 


20.9 


0.0891 


40.0 


0.1131 


80.8 


0.0976 


40.90 


0.1051 



HYDROGEN I 



SOLUBILITY OP HYDROGBH IN SEVERAL SOLVFMTS. 

and Moon, 1936,) 



Some of the determinations were made with an apparatus with a mag- 
netically operated stirrer such as employed by Horiuti. For the others 
a form of apparatus which permitted stirring by rocking the mixture was 
employed. 



\cetic Acid 



Ethyl Alcohol 



Ethyl Acetate 



Chloroform 



Benzene 



t 


at Solution 


(nun Hg)of Solvent 


expressed as 




Temp. 


at Solution Temp. 


Bun a en Abe. Coef. 


18.6 


1.0507 


11.0 


0.05S8 


20. O 


1.049 


12.0 


0.0566 


30.0 


1.039 


21.0 


0.0594 


37.5 


1.031 


30.0 


0.0620 


45.0 


1 .023 


45-0 


0.0649 


54.9 


1.011 


72.0 


0.0676 


6/1.8 


1 .000 


109.O 


0.0714 


74-3 


0.989 


l66.O 


O.0742 


0.6 


0.8063 


12.2 


0.0718 


10.0 


0.7978 


2 3 .8 


0.0737 


20.3 


0.7890 


44-0 


0.0769 


25-0 


0.7851 


6o.O 


0.0784 


30.0 


0.7808 


78.0 


0.0802 


40.0 


0.7730 


133-0 


0.0840 


50.O 


0.7633 


220.0 


0.0864 


0.5 


0.9244 


25.0 


O.0708 


10. O 


0.9126 


42.7 


0-0724 


21.0 


0.8993 


76.9 


O.076l 


30.0 


0.8883 


118.7 


O.o8o8 


39.8 


0.8762 


184.0 


0.0803 


1.0 


1.5260 


6l.O 


0.0563 


10.0 


1.5050 


100.0 


0.0576 


18.7 


1.4886 


149-6 


0.0584 


25.5 


1 .4750 


197-0 


o . 06 l a 


0.5 


o . 900 i 


25-0 


0.0526 


8.3 


0.8920 


43-0 


0.0572 


21.2 


0.8775 


79-0 


0.0625 


30.6 


0.8675 


123.0 


0.0672 


40.0 


0.8576 


l8l.l 


0.0727 



H HYDROGEN 



566 



HYDROGEN 



SOLUBILITY OF HYDROGEN IN SEVERAL SOLVENTS. 

(Klrjeew and Romantchonlc, 1936.) 
Total Oas pressure cc H g (reduced to o and veomm^dlssolved fry i cc Solvent at: 



In iw. HR. 



-10 



420 



Petrol (Gasoline?) 


50 


0.010 


0.008 


O.007 


0.005 


0.004 


H 


100 


0.019 


0.0l6 


0.014 


0.010 


0.008 


n it 


200 


0.038 


0.034 


0.028 


0.021 


0.017 


ti n 


300 


0.056 


0.051 


0.043 


0.033 


0.025 


n n 


400 


0.074 


0.068 


0.057 


0.044 


0.034 


M It 


500 


0.092 


0.085 


0.072 


0.054 


0.042 


tt n 


600 


0.111 


0.1O2 


0.087 


0.065 


0.050 


ti ft 


700 


0.129 


o. 119 


0.101 


0.076 


0.058 


II H 


760 


0.140 


0.129 


0.110 


0.083 


0.064 


Xylene 


50 


0.006 


0.005 











tt 


100 


0.013 


0.011 


0.009 


0.009 


0.010 


n 


200 


0.026 


0.024 


0.018 


0.018 


0.021 


n 


300 


0.039 


0.036 


0.029 


0.029 


0.033 


" 


400 


0.052 


0.048 


0.039 


0.039 


0.044 


it 


500 


0.065 


0.060 


0.046 


0.049 


0.056 





600 


0.078 


0.072 


0.059 


0.059 


0.067 


n 


700 


0.091 


0.084 


0.069 


0.069 


0.078 


it 


760 


0.099 


0.091 


0.075 


0.075 


0.085 


tracking Benzene*??) 


50 


0.014 


0.012 


0.010 


0.008 


0.005 


n H 


100 


0.028 


0.022 


0.018 


0.016 


0.010 


H II 


200 


0.058 


0.044 


0.036 


0.030 


0.020 


" " 


300 


0.087 


0.064 


0.056 


0.044 


0.030 


tt II 


400 


0.116 


0.084 


0.074 


0.059 


0.040 


II II 


500 


0.146 


0.105 


0.094 


0.074 


0.051 


II II 


600 


0.175 


0.126 


0.112 


0.088 


0.061 


n it 


700 


0.202 


0.148 


0.132 


0.102 


0.072 


n it 


760 


0.220 


o. 160 


0. 144 


0. Ill 


O.Q78 



Results are also given for Dichlor Ethane and "Heavy Solvent" which are- 
fairly near those for "Cracking Benzene" at 20. 

i liter Cyclo hexanol (C e n tl pH)dissolve 83.100 H g at 20 and 7601 pressure. 

(Cauquil, 1927.) 



567 HYDROGEN H 

SOLUBILITY OF HYDROGEN IN SEVERAL SOLVENTS AT 25 AT HIGH PRESSURES. 

(Frolicft, Touch, Mogon and per, 19?JI.) 



The determinations were made by shaking the solvent with various pres- 
sures of hydrogen in a steel cylinder maintained at 25, and, after attain 
ment of equilibrium, withdrawing a sample of the saturated solution over 
mercury, in a buret designed so that the volumes could be measured with 
the same decree of accuracy at any ratio of #as to liquid. The results 
are presented in the form of a diagram from which the following approxi- 
mated values were estimated. 

cc Hg (measured at . 8 And 7600w> dlasolvta t>y l.Occ flolwnt &ti 
Solvent -To ~~~~ -gQ"~-- 80 10 Q ^'"'At' 

Methyl alcohol 3.3 $.0 7.0 8.5 ia-5 

Propane 17.3 25.0 34.0 42.5 

iso Propanol 2.5 4.5 6.0 7$ 11.3 

Pentane 9.0 13.5 18.2 22.5 

Butane n.o 16.5 22.0 27.0 

Hexane 5.0 11.0 i$.o 18.0 

Octane 6.0 8.$ **-S i*J-9 22.0 

Cyclohexane 4.0 6.0 8.0 60.0 15.2 

Heavy Naphtha 2.7 4.3 $-6 7.3 U) ,B 

Gas Oil 2.5 4.0 $.3 6.8 *o.Q 



DATA FOR THE SOUTH XMTY or HYDROGEN IN THE FOLLOWING MITALS 
HAVE BERN DKTKHHINKO. 

AU (St<*acie and Johnson, 1928.) Mo (Martin, 1929.) 

Ce (von Samson-Kimmelstjerna, 1930. )Nb (Hagen and Sif-verts, 1930.) 

Co (Sieverts, 1907; Sicverts and Ni (Si averts, 1911; Luckemeypr 

Hagen r 1934.) Hasc and Shenk, 1932.) 

Or (Martin, 1929; Tamman, 1930; Pd (Si everts, 1914; von 
Luckemeyer-Hasse and Shenk, Himmel^tjerna, 1930," 

1932.) and Zapf, 1935 ^l?w 

Cu I Si everts, 1911.) suits for the Solubility of 

Fe (Sieverts, 1911; Martin, 1929; Deutoriutn. ) 

Sieverts and llaf;en, 1931 Pt (Sieverts and Jurisch, 19131, II 

Luckemeyer-Hasse and Shenk, Ti (Ha^n and Sievert, J93DJ 
1932.) Kirschfeld and Si^v^rts, 

(Sieverts, Zapf and Moritz, 1938.) V (Kirochf^ld and Sieverts, 

Ge (Hagen and Sieverts, 1930.) ^ 1930.) 

In I ! " V (Martin, 1929,1 

La (von Samson-HimmelsT j^rna, 1930.) 
Mn (Luckemeyer-Hasse and vSchenk, 1932.) 

HYDROGEN BOKATE H^HO^ (See Boron Oxide Hydrate* 
HYDROGEN BROMIDE ( Hydrobromu 1 Acid) HBr 



H HYDROGEN 568 

HYDROGEN BROMIDE 

SOLUBILITY IN WATER. 

(Rooeeboom Z, pfcysik. Chem. 2, 454. '88; Rcc. trav. chim. 4, 107, '85; 5, 358, '86; see also Pickering 
Phil. Mag, [5] 3<5 ii9, '93-> 

GmsJHBrDissolved(at76o-765mm.) Cms. HBr Dissolved at 

*.* Per I0 Gms. o Lower Pressures per 100 

* ' Gms.H 2 O. 

175.0 (10 mm.) 
108.5 (5 mm.) 





" Water. 


Solution. 




- 2-S 


255-0 


71.83 





I 


239.0 


70.50 




O 


221.2 


68.85 


611.6 


+ 10 


210.3 


6 7 . 7 6 


581.4 


15 


204.0 


67.10 




25 


193.0 


65.88 


532.1 


5 




63.16 


468.6 


75 


ISO'S 


60.08 


406 . 7 


TOO 


130.0 


5 6 -5 2 


344-6 



ft - Bunsen Absorption Coefficient which is the volume of gas (reduced 
to o and 76omm) absorbed by i volume of the liquid wlien the pressure 
of the gas itself, without the tension of the liquid, amounts to 76omm. 

EQUILIBRIUM IN THE SYSTEM HYDROBROMIC ACID, VATBR AND ALCOHOLS AT 25. 

(Return and Shearer, 1933.) 

The determinations were made by adding from a buret one of the consti- 
tuents to known mixtures of the other two until appearance of permanent 
turbidity. The tie lines of the saturation curve thus obtained were de- 
termined by mixing suitable amounts of the three constituents to yield 
two liquid layers at 25 and titrating each of these for HBr content. 

Results for IIBr + HO . Results for HBr * H 2 

+ Iso Amyl Alcohol, (CH S ) 2 CHCH 8 CH 2 OH + Iso Butyl Alcohol, (CH 3 ) 2 CHCH 2 OH 

tea. per 100 Ons. per 100 

y. aol. gma. a^t. aol. 





9.0 


91.0 


42.0 25.0 


l6.1 83.0 


62.4 2O. 





11.36 


85.3 


45.8 19.1 


22.6 72.7 


66.9 15. 


4 


16.90 


76.8 


54.7 


8.17 


29.1 61.8 


70.8 12. 


6 


17.7 


70.6 


67.7 


3.39 


35-1 53.1 


75-5 11- 





21.2 


63.2 


76.9 


3.00 


48.9 35.0 


82.8 8. 


7 


26.4 


57.6 


83.0 


2.84 


57.3 25.7 


91.2 . 8. 


8 


28.4 


47.8 


9L7 


2.58 








30.2 


44.2 


97.0 


3.00 










Tie 


Line Data 




Tie 


Line Data 




Qftia. HBr j$r 100 918. 


OMa. HBr Pfr 100 gma. 




jO layer 


CJLgO layer 


H g O layer 


C 4 H 10 layer* 




13 


5 


3.5 




10.8 


6.0 




24 


.0 


13-0 




8.7 


4-3 




34 


.1 


23-5 











569 HYDROGEN II 

a- POINTS OP DILTJTB AQUBOUS HYDROBROMIC ACID SOLUTIONS. 

(Klein and Svanberg, 1920.) 
t of F. pt Nonnallty of Aq. HBr 

-0.362 o.i 

-0.923 0.25 

-1.907 0-5 

fcYeez ing-point data are given for mixtures of HBr and each of the 
flowing compounds. 

l ,0fl (1) <C g H 5 ) 2 (3) C 6 H 5 C 2 H 5 (2) 

iR-OH (i) C 3 !L (4) C 6 H 5 C 3 H 7 (5) 

'!:C!I (2) CH 3 COCH 3 d) C 7 H 4 (5! 

d) CH 3 COOC 2 H 5 d) C 6 H 4 (CII 3 } 2 o m (5) 

(i) C 6 H 6 d) C 9 H 12 < 2 )~ 

d) CejHgCHg (i)(2) H 2 S (6) 

C 6 H 3 (CH 3 ) 3 (s)( 2 ) 

(i) = Maass and Mclntosh, 1912; Reid and Mclntosh, 1916; (2) = Maass and 
'^sell, 1918; (3) McTntosh, 1911; (q) Maass and Russell, 1921; (5) Maass, 
'%er arid Morrison, 1.923," (6) Ragster, 1911. 
r )ROGBN CYANIDE HCN 

CN 
FRKRZING-POINTS OF MIXTURES OP HYDROGBN CYANIDB AND WATER. 

(Coatea and Hartshorne, 193 i.) 

The apparatus was provided with a magnetically operated stirrer. A 
"cury thermometer was used and the freezing-points determined by back 
: rapolation of time-temperature curves over the super cooling region 
ept near the eutectic point. Here it was necessary to employ a jet 

sir directed a short distance above the level of the liquid. The rapid 
Lporation thus induced caused crystals to form which inoculated the mix- 
*e and prevented super coolinp,. The mixtures of which the freezing- 

nts were determined were analyzed by Liebig's method of silver nitrate 

ration. The results in the metastable region were obtained by a modi- 
l d form of apparatus in which stirring was avoided and a rapid rate of 
ling was employed. 

to. M01S. HCN SoH(J <ta. Hols. HCN ^^ fa. Mols. HCN 8olw 

: per 100 n. Mola. phase t per 100 gm. Mola. phase t per 100 pi. Mola. ^^ 
HCN HgO HCN * HgO HCN * H 

>.9 0.81 Ice -16. q 50.29 Ice -15.8 95.9 HCN 
3.5 3^09 " -17.3 59.24 " -14.4 98.5 " 

7.7 7.76 " ~39.3 66.96 " "13.3 10O.O " 

>.9 9-89 " -21.1 70.4 " -24.7 24.8* 

, .8 14.25 " -22.6 73-0 " -24.0 34.4* 

^4-5 19.36 " -23.4 74.5 " + HCN-24-1 39.2* 

;.5 26.29 " -22.5 79-7 HCN -24.5 47.9* 

,.0 36.82 " -19.4 ^3.9 " -25.6 54-7* 

-27.5 58.7* 

Metastable region - consisting of two liquid phases with critical 
ution temp, of -24.0. 

dditional determinations in agreement with the above are fjiven by 
K-er and Coffiff, 1933. These investigators also give results for the 
pts. of mixtures of HCN * HCOOH, HCN * HCONH ? and HCN 1 * C fl II g CHO. 



H HYDROGEN 



CN 



570 



HYDROCYANIC ACID HCN. 

DISTRIBUTION .BETWEEN WATER AND BENZENE. 

(Hantzsch and Scbalt, 1899; Hantzsch and Yagt, ryoi.) 



Mol. HCN per Liter: ^ 

HjO Layer (<;). QHe Layer (c 1 ). / 

6 0.00625 0.00325 1.923 
16 0.00593 o-3 6 3 1-634 

25 0.00580 0.00375 1-547 



Moi. HCN per Liter: c 

' HO Layer (c). C 8 H fi Layer (<;'). ?* 

7 0.0574 0.0148 3.88 

20 0.0572 0.0154 3.72 



Data for the effect of HC1 and of KC1 on the distribution are also given. 
DISTRIBUTION OP HYDROGEN CYANIDE BETWEEN WATER AND BENZENE. 



(Gross and Schwarz, 1930.) 



15 



On. Mols. HCN 


^per lOOOcc: 
layer 

0.002665 
0.005342 

0.01073 
0.05916 
0.0749 
0.0828 


' V 

layer 

0.01084 
0.02167 
0.04334 
0.2321 
0.2905 
0.3214 



15 



(*. Mols. HO 


jf^per IQOOcc; 
layer 


layer 


0.3494 
0.3777 


0.0905 
0.0981 


0.3999 


0.1051 


0.4740 
0.4830 


0.1254 
0.1275 


0.4933 


0.1307 



(3m. Mols. HCN^per lOOOcc: 



15 



8.0 
8.3 
8.3 



layer 

0.5532 
0.6507 
0.9178 
0,4123 
0.4203 
0.7789 



layer 

0.1486 
0.1772 
0.2598 
0.1053 
0.1079 
0.2089 



The authors also give results for the distribution of HCN at 15 between 
Benzene and aqueous solutions of KC1, KN0 3 , CsN0 3 , NaN0 3 , LiN0 3 , urea and 
glycerol. Results are given by Gross and Iser, 1930 for the distribution 
of HCN at 15 between Benzene and aqueous solution^ of LiCl, NaCl, NaNO , 
K 2 S0 4 , MgCl g , MgS0 4 and La g (SO ) . Results are given by Randall and Halford, 



1930, 



for the distribution of 



tions of Hydrogen Silver Cyanide (HAg(CN) ). 



at 25 between Benzene and aqueous solu- 



HYDROGEN CYAN ATE (Cyanic Acid) HCNO 

SOLUBILITY OP HYDROGEN CYANATE IN WATER DETERMINED 
BY THE FREEZING-POINT METHOD. 

CNO (Llnhard, 1938.) 

Although cyanic acid decomposes in presence of water it was found 
that mixtures of the two are stable at sufficiently low temperatures 
and the following results were obtained for the freezing-point curve. 



t(cor.) 

-23.5 
-28.7 
-33-7 
-39-6 
-42.2 
-50.0 
-62.0 



Mols. HCNO per 
100 Mols. HCNO Hg 

29-3 
33-3 
38.3 
43-2 
45-0 
49-8 
55-3 



Solid 
Phase 



Mols. HCNO per 
t (cor.) 1QO Moig ^ HCNQ ^ j. 


I -68.8 
-83.6 
-102.5 Eutec. 
-101.0 


58.5 
62.8 
67.0 
68.1 


-97.2 
-93-2 

-86.8 . pt. 


74-9 
83.6 
100.0 



aollci 
Phase 



H ? 



HCNO 



HCNO 



57i HYDROGEN H 

HYDROCHLORIC ACID HCL 

SOLUBILITY IN WATER BY THE FREEZING-POINT METHOD. 

(Composite curve from results of Roloff, 1895; Pickering, 1 893 (a); Roozeboom, 
1884, 1889 and Rupert, 1909.) 



Gms. HC1 
t. per 100 Gms. Solid Phase. 


Gms. HC1 
t. per 100 Gms. Solid Phase. 




Sat. Sol. 




Sat. Sol. 




1 . 706 


1 . 66 Ice 


18.4 


48.6 


HC1. 2 H 2 O 


~I4.97 


IO.O2 


17.7 m. pt. 


50.3 


" 


-28,84 


I4-5 1 " 


-18.7 


52.85 


" 


-40 


17.40 


-19.4 


54-1 


" 


-60 


21.30 " 


-20.8 


55-7 


" 


-80 


24.20 " 


-21.3 


56.5 


" 


-86 Eutec. 


24.8 ' +HC1. 3 H 2 


-23.2 


57-3 





50 


30.1 HC1.3H 2 


23 . 5 Eutec. 




" +HC1.H 2 


-40 


32.7 


-21.5 


58*2 


HC1.H 2 


30 


36.5 




59-i 


" 


24 . 9 m. pt. 


40.3 


18.4 


61.1 


" 


-27.5 


44 " +HC1. 2 H 2 


-17.4 


62.4 


" 


-23.8 


45.7 HC1. 2 H 2 


"""" ^5*4 


65-4 


* 


21 .2 


45-9 


-iS-35 


66.8 


" 



At about 15.35 two liquid layers are formed. Data for these are as follows: J 



HC1 layer. 

A^ 


fof JJ^-% 
Saturation P S nt <^ 


Below 50 


0.008 


" -So 


0.017 


Bet. -15 and o 


0.077 


Above 45 


0.021 


" 


0.052 


" 


o.ir 


" 


0.13 



H 2 layer. 



20 
-IS 

-5 
o 

+5 

IO 



Gms. HC1 

6*7.65' 
67.29 
66.71 
66.44 
65.85 
65.48 
65.18 



d. of Sat. Sol. t. 



1.279 
1.269 
1.260 

1-255 
1.247 
1.245 
1.240 



15 

20 

30 
35 
40 

45 
50 



Gms. HC1 

per loo Gms. d. of Sat. Sol. 
Sat. Sol. 
64.70 
64.19 
63.21 
62.90 
62.27 
61.76 



61.65 



.231 
.228 
.229 
.227 
.218 

I. 212 
I.2IQ 



For additional data on this system see Baume and Tykociner, 1914. 

FREEZING-POINTS OP DILUTE AQUBOUS HYDROCHLORIC ACID SOLUTIONS. 

(Chadwell, 1927.) 

The determinations were made with the highest possible precision. A 
platinum thermometer and Wheatstone bridge were used for measuring the 
temperatures. The analyses were made upon solutions in contact with a 
large amount of added ice. 



F. pt. lowering 
below o C 

-0.2934 
-0.5033 
-0.7145 
-0.7771 
-0.8440 
-1 .1000 
-1.1202 
-1.4738 
-1.9344 



Om. Equlv. HC1 



0.08321 

0.1427 

0.2024 

0.2198 

0.2374 

0.3080 

0.3137 



P. pc. lowering 
below o C 

-2.3664 
-2.5465 
-2.6114 
-2.9420 
-3.1219 
-3-4545 
-3.8192 
-4.0721 



0.5275 



Om. Equlv. HC1 
per 1000 gms. H g O 

0.6363 
0.6785 
0.6969 
0.7736 
0.8l87 
0.8945 
0.976s 
1.0324 



A compilation of the available data upon the partial vapor pressure of 
aqueous solutions of hydrochloric acid is given by Zeisberg, 1925.) 



H HYDROGEN 572 

FREEZING-POINTS OF DILUTE AQUEOUS HYDROCHLORIC ACID SOLUTIONS. 

(Klein and Svanberg, 1920.) 



t of F. pt. 



Normality of HC1 



Cl 



-0.34 

-0.876 
-1.807 

HYDROCHLORIC ACID 



o . i 

0.25 
0.5 



HC1. 



SOLUBILITY IN WATER AT DIFFERENT TEMPERATURES AND 
PRESSURES. 

(Deicke; Roscoe and Dittmar Liebig's Ann. 112, 334, 59; below o, Roozeboom Rec. trav. 

chini.3, 104, '84.) 

At Different Temperatures and 760 mm. Pressure. At Different Pressures and o 



f. 


cc. HClper 
loocc.HaO. 


D"** G I oo s g H s!>r 


Gms. HC1 per 
100 g. EkO. 


Pressures.* 


?r g H Ha 





525.2 


1.2257 


45-15 


82.31 


60 


6i'-3 


4 


497 7 


1.2265 


44 -3 6 


79 73 


100 


65-7 


8 


480.3 


1.2185 


43 83 


78.03 


150 


68.6 


12 


471 .3 


1.2148 


43-28 


76.30 


2OO 


70-7 


14 


462 4 


1.2074 


42.83 


74.92 


300 


73-8 


18 


451 .2 


i . 2064 


42.34 


73-4i 


400 


76-3 


23 


435-0 


1.2014 


41*54 


71.03 


500 


78.2 


30 






40.23 


67-3 


6OO 


80.0 


40 






38.68 




750 


82.4 


So 






37-34 


59-6 


IOOO 


85.6 


60 


... 


... 


35-94 


56.1 


1300 


89-5 



100 gms 
gm. at 25. 
loocc sat. 



* Pressures in mm. Hg minus tension of HaO vapor, 
sat. sol. of HC1 in H 2 contain 45.44 gm. 



(Cupr, 1926, 1928. ) 



sol. of HC1 in H g O contain 71.9 
Hiashelwoort, 1927.) 



HC1 at o 
HC1 at 20. 



and 41.2 
t Knight and 



SOLUBILITY IN WATER AT TEMPERATURES BELOW o. 



At a pressure of 760 mm. At pressures below and above 760 mm. 



t. 


Q- 


t. 


Q- 


t. 




mm. Pressure. 


$ 


24 


IOI .2 


-*5 


93-3 


-23 


.8 




84.2 


21 


98.3 


10 


89.8 


21 




334 


86.8 


18.3 


9 6 


- 5 


86.8 


~I9 




580 


92.6 


18 


95-7 


o 


84.2 


-18 




900 


98.4 










-17 


7 


1073 


101.4 



The eutectic is at 86 and 33 gms. HC1 per 100 gms. H 2 O. 

f = the weight of HC1 gas in grams dissolved by 100 grams of H g O at the 
indicated temperature and at a total pressure (that is the partial pressure 
of the gas plus the vapor pressure of the liquid at the absorption tempera- 
ture) of 76omm.Hg. 

Data for the solubility at 25 of HC1 gas in water at low pressures are 
given by Dobson and Masson, 1924. 



573 HYDROGEN H 

SOLUBILITY OF HYDROCHLORIC ACID GAS IN AQ. SULFURIC ACID SOLUTIONS. 

(Coppadoro, 1909.) 



Results at 17. 

Gms. per too Gms. 
dofjat. Sat. Sol. 


Results at 40. 

. Gms. per 100 Gms. 
d oj_Sat. Sat. Sol. <* < 


Results at 70. 

r ,_ Gms. per 100 Gms. 
g Sat. sat. Sol. 


" 


H 2 S0 4 . 


HCL 




H 2 S0 4 . 


HCl. ' 




. 


' H 2 S0 4 . 


HCl/ 


I. 211 


o 


42- 


7 


I 


.185 


3-56 


35-6 


i 


145 


1.61 


32.7 


I .220 


1.86 


39- 


9 


I 


-195 


5.86 


34-8 


i 


.150 


3.38 


31 .1 


I .220 


4-75 


39- 


,2 


I 


.2IO 


8.90 


32.4 


i 


.160 


4.80 


30 ..5 


1-235 


8.04 


36- 


9 


I 


-255 


16.80 


27.6 


i 


.180 


7-93 


28.9 


I .260 


12.80 


33- 


,2 


I 


-255 


18.8 


25-9 


i 


.225 


18.9 


22.8 


i -3S 


20.9 


28. 


5 


I 


.340 


28.6 


I8. 5 


i 


.230 


20 


22.3 


1-355 


30.8 


22. 


.6 


I 


.400 


44-2 


"5 


i 


315 


36.2 


13.2 


1.430 


44-6 


15 




I 


520 


6i.r 


3-35 


i 


.380 


48 


6.99 


1-545 


59-4 


6 


.26 


I 


575 


66.4 


1.17 


i 


.510 


62.7 


1-56 


1.580 


65.4 


3 


25 


I 


-650 


73-2 


0.17 


i 


.560 


67.6 


0.54 


i. 660 


73-7 


o 


.62 


I 


725 


79-4 


0.081 


i 


.700 


80.7 


0.05 


1-735 


77-5 


o 


.11 


I 


-755 


81.4 


0.032 


i 


-745 


83 


0.035 


1.815 


89 


o 


.068 


I 


.770 


83-5 


0.029 


i 


-745 


83-4 


O.O32 



SOLUBILITY OP HYDROCHLORIC ACID IN CONCENTRATED SULFURIC ACID 

AT 25 AND 76omm. Cl 

(Cupr, 1925.) 

percent OB. HCl per 100 Percent On. HCl per 100 percent OB. HCl per 100 
H SO. gws. sat. sol. H S0 4 BS * aat> so1 * H 2 80 4 8Wfi " 8at; * 8o1 " 

76. (|3 0.3588 90.69 0.0922 97.36 0.1432 

8l.87 O.lq.20 92.20 0.0996 98.65 0.1971 

86.76 0.0974 94-14 0.1082 100.00 O.4015 

89.31 0.0920 

Additional determinations at other temperatures and concentrations of 
H g SQ 4 are given by Cupr, 1925 (a), 1928. 

SOLUBILITY OK HYDROCHLORIC ACID IN AQUEOUS SOLUTIONS OF ACETIC ACID. 
Results at o < Capr ' 1926 - 1928 -> Results at 25 



Gma. .CH^COOH 


Oms. HCl 


cc HCl gas per 


Dros. CH_COOH 

<3t 


Oms. HCl 


cc HCl gas per 


per 100 gms. 


per 100 gms. 


l.Occ sat. sol. 


per 100 gma. 


per 100 gma. 


l.Occ sat. sol. 


aq. Solvent 


aq. Solvent 


at 760mm 


aq. Solvent 


aq. Solvent 


at 7GOmm 


11.52 


76.<1 


479.2 


11.02 


63.03 


390.2 


19.03 


72.72 


461.2 


22.90 


55-45 


349.8 


27.96 


66.98 


430.8 


33.69 


51.06 


325.8 


48.89 


55.69 


366.6 


48.38 


42.67 


275-7 


72.96 


41.41 


276.7 


70.95 


30.66 


200.4 


79.86 


37.51 


251 .0 


87.04 


21.32 


139.1 


89.56 


31.48 


210.3 


95-24 


14.13 


91.5 


89.49 


31.39 


209.0 


99-45 


8.35 


53.6 



MISCIBILITY OF HYDROCHLORIC ACID WITH MIXTURES OF WATER AND 
PHENOL AT 12. 

(Schreine makers and van der Horn van dcr Bos, 1912.) 

Composition of the Reciprocally Composition of -the Solutions in 

Saturated Liquid JPairs. Contact with Solid Phenol. 

Water Rich Layer. 

%HC1. % Phenol. 

o 7-45 

3.1 6.6 
6.6 5.3 

8 5-1 

10.7 4.8 

Additional data for this system are given by Krug and Cameron, 1900. 



% HCl. 


% Phenol'. 


% Water. 


% HCl. 


%' Phenol. 


O 


72 


11.22 


O 


88.78 


O.OQ 


78 


84.5 


I0.y 


4.8 


O.2 


80.3 


80.38 


15-6.4 


3-98 


0.36 


82.6 


72.43 


24-37 


3-2 


0.52 


84.5 


00.25 


36.25 


3-5 



H HYDROGEN 



574 



HYDROGEN CHLORIDE 

EQUILIBRIUM IN THE SYSTEMS HYDROCHLORIC ACID, WATER AND ORGANIC SOLVENTS. 

(Re burn and Shearer. 1933.) 

The determinations vrere made by adding from a buret, one of the consit- 
tuents to known mixtures of the other two until appearance of a permanent 
turbidity. The tie lines of the saturation curve thus obtained were de- 
termined by mixing suitable amounts of the three constituents to yield 
two liquid layers and titrating each of these for acid content. 

Results at 25 for HCl 4 Results at 25 for HCl+Results at 25 for HCl* H/) - 



Cl 



HO + Iso Amyl Alcohol 
((CH 3 ) ? CHCH 2 CH 2 OH) 



H + Iso Butyl Alcohol 
( (CH 3 ) 2 CHCH 2 OH) 



Cyclohexanone 



ttns. per lOO^gms. sat; sol. 


Qns. per lOO^gms. sat. sol. 


Gms. per 100 gms. sat. sol. 


' H 2 C 5 H 12 


' H 2 C 4 H 10 N 


/ U f) f> rt ~\ 

H 2 C 8 H 10 


8.9 91.1 


16.1 83.9 


7.5 92.5 


14.15 82.7 


27.3 68.4 


22.1 74.4 


18.90 74.6 


35-4 58.3 


34*6 59-8 


23.10 67.7 


40.0 52.3 


43-4 49-6 


38.8 44.1 


44-6 46.6 


50. -2 41.9 


49.5 29.8 


49.6 40.0 


54.4 36.9 


54-3 23.6 


53.2 36.7 


56.5 34-0 


64.9 11.3 


59-2 30.0 


62.8 27.0 


72.0 5.l6 


69.5 18.7 


68.1 21.7 


83.6 3.60 


79.8 10.3 


72.8 17.2 


91.4 2.79 


84.8 8:4 


81.4 12.3 


97.1 2.90 


91.2 8.8 


87.8 12.2 


Tie Line Data 


Tie Line Data 


Tie Line Data 


Ins. HCl per 100 gms. 


flms. HCl per 100 0ns. 


Ons. HCl per 100 gms. 


HgO C & H lg O v 


' H 2 <VlO ^ 


H 2 C 6 H 10 


layer layer 


layer layer 


layer layer 


7.83 1.99 


10.4 6.3 


9-5 2.3 


16.13 7.30 


7.7 3.6 


8.8 1.1 


21.7 14.7 


4.2 1.3 




Results at 40 for 


Results at 55 for 


Results at 25 for 


HC1+H ? + Iso Butyl 
Alcohol '((CH.KCHCH. OH) 

c c f. 


HC1 + H + Iso Butyl 
Alcohol ((CH,).CHCH,OH) 

Of, , 


HCl 4- H + n Butyl 
Alcohol (CH.iCL^CH.OH) 

O f. K, f, 


Qms. per 100 gns. sat. sol. 


Ctas. per lOO^gms. sat. sol. 


Qms. per 100 gms. sat. sol. 
x\ 


H C.H..O v 


' H rt O C.H.^0 N 




2 4 10 


Z 4 10 


?. 4 10 


17.9 82.1 


21.8 78.2 


21.9 78.1 


26.6 69.6 


29.2 67.2 


29.2 67.1 


42.6 ' 49.3 


37.0 56.8 


39-7 54-3 


53-5 36.9 


50.6 40.5 


51-9 39-4 


64.0 25.0 


64.3 24.8 


66.4 23.3 


74.0 14.7 


72.4 16.6 


75.4 13.9 


8l.2 10.0 


80.7 10.5 


84.9 8.5 


92.0 8.0 


91.2 8.8 


91.7 8.3 



575 HYDROGEN H 

DISTRIBUTION OF HYDROCHLORIC ACID BRTWBBN WATER AND BRNZBHE. 



Results at 20 

(Knight and Hinshelwood, 1927.) 



Results at 25 

(Wynne-Jones, 1930.) 



Oms. HCl per lOOOcc Oms. HCl j?er lOOOcc Oms. HCl ^er lOOOcc Pro. Mols. HCl ^per 1000 gas.; 



H 2 


C 6 H 6 ' 


' HgO 


c e H e % 


' HgO 


_ s , 


V 


CgH e 


layer 


layer 


layer 


layer 


layer 


layer 


U/er 


layr 


718.8 


18.50 


420.2 


2.47 


212.0 


0.252 


9.603 


0.00213 


604.0 


17.7 


379.8 


1.818 


165.9 


0. 100 


10.215 


O.OO340 


549.3 


17.4 


343-3 


1.264 


134.0 


0.056 


10.508 


0.00423 


509.0 


15-7 


312.0 


0.929 


94.8 


0.028 


11-43 


O.OO768 


504.6 


15.62 


289.3 


0.706 


43-3 


0.0036 


11.99 


0,0110 


492.5 


8.92 


259.0 


0.532 


19-5 


O.O002 


12.93 


0.0216 


448.5 


3.72 


236.1 


0.382 


12.3 


0.0001 







looocc pure benzene dissolve 16.8 gm. HC1 at 20 and 76omm pressure. 



looocc pure benzene dissolve 16.8 gm. HCl at 20" and 76omm pressure. 

looocc benzene previously saturated with H 2 dissolve 18.31 gms. HC1 at 
20 and 76onim. 

looocc benzene simultaneously saturated with H 2 and HC1 dissolve 18.50 
gms. HC1 at 20 and 76omm. ' "-'--*- J ..,__,.-,...-, , 



(Knight and Hinshelwood, 1927.) 



DISTRIBUTION OP HYDROCHLORIC ACID BBTWBBN WATER AND NITRO BBNZBNB AT 25 



Ow. Mols. HCl per 1000 gms. 



(Wynn-\Jones, 1930.) 
On. Mols. HCl per 1000 



Cl 



0m. Mols. HCl per 1000 gwa. 



HgO layer 


C 6 H 5 N0 3 layer 


9.635 


O.0027 


11.147 


0.0080 


11.6l 


0.0109 


12.84 


0.0229 


13.34 


0.0396 



14.84 
15.21 
16.46 
17.19 
17.76 



0.0707 

0.0833 

0.164 

0.223 

0.292 



\ Z layer 


W3 Uy * r 


18.05 


0-335 


18.38 


0.394 


19.33 


0.556 


19.52 


0.603 


20.42 


0.833 



Data have also been determined for the Distribution of HCl between H g O 
and each of the following compounds at 25: Amyl Alcohol, Tertiary Amyl 
Alcohol, n Butyl Alcohol and Methyl Rthyl Ketone (Archibald, 1932.) 

Results for the distribution of HCl between H 2 and Phenol are given by 
Wosnessensky and Astachow, 1925. 

SOLUBILITY OF HYDROCHLORIC ACID GAS IN METHYL ALCOHOL, ETHYL 
ALCOHOL, AND IN ETHER AT 760 MM. PRESSURE. 

(cte {Jruya - Rec. tray, chiin. n, 129, '92; Schuncke Z. physik. Chenv. 14, 336, '94.) 
Grams HCl gas per 100 Grams Solution in: 



IO 

- 5 

O 

+ 5 
10 

IS 

20 
25 
30 



CHsOH. 
54.6 

51-3 



47-0(18) 



C 2 H fi OH. 


(C 2 H fi ) 2 0. 




37-5 1 (- 




37.0 


45 '4 


35 -6 


44-2(6.5) 


33-1 


42.7(H'5) 


3 35 




27 .62 


41.0 


24.9 


40.2 (23.5) 


22.18 


38.1 (32) 


J9-47 



H HYDROGEN 576 

FREEZING-POINTS OF MIXTURES OF ETHYL ETHER AND HYDROCHLORIC ACID. 

( Hirai, 1926. ) 

per joo*mols. Solid per 100 mils. Solid 

t. sat. sol. Phase. t. sat. sol. Phase. 

-117.7.. ioo. o (G. 2 H 5 ) 2 -87.4 36.*9 (C 4 H 5 ) 8 Ol(HCl), 

n8.-8,. 89.16 87.3in.pt.. 33.33 

119.3.. 86.(j3 89.0 31.70 

124.2.. 79-68 ( .)3-5 27- 3c) 

127.8.. 77.33 100.4 ai.ofi 

126.6.. (58.o4 (CH 5 )sO.(HCI)i 104.0 18.76 

ii5.4.. a3. 66 u3.) ii. ao 

no. q.. ,)Q.5) n5.5 io.55 

- - - 3.6 6.08 



-100.9.. 50.97 
-107.3.. 47.18 



123.7 5-7.0 HCl 

1 20 . H 4-^5 

i2O. r > 3.87 > 

I 12.5 O.OO 



The following determinations by Mclntosh, 1928, differing from the above 
were made in a specially constructed freezing-point apparatus provided 
with a magnetically operated stirrer and a very accurate platinum quartz 
thermometer. 

Mol. Percent Solid Mol. Percent Solid 

l HC1 Phaae r HCl Phase 

-102.9 42.5 (C 2 H 5 ) 8 O.HC1 -84.8 70.0 (C E H 6 ) 2 0.2HC1 

-100. 47.3 n -97.6 71.6 " " 

-98.6 50.0 " -99.6 80.5 (C 2 II 5 ) 2 0.sHCl 

-97.9 54.2 " -96.2 81.5 " 

-100.^ 56.5 " -92.9 83.6 " 

-82.0 65.6 (C H ) 0.2I1C1 -94.2 85.0 

-83.2 67.6 

FIBRZING-POIRTS OF MlXTURKS OP HYDROCHLORIC ACID AND ACRTONB. 
(Hlral, 1926: Mclntosh, 1928.) 

Moi perceat Solid Mol. Percent Solid 
1 HCl Phase l HCl Phase 

-94-5 o.o CCH ) CO. -84.6 57-7 (CfL I.CO.HCl 

-107.0 14.43 (CH 3 ) ? CO.HC1 -82.7 55.56 " 

-11^.6 27.29 " -86.6 57.26 " 

-91.5 36.5 " -92.8 60.39 " 

-85-7 42.99 " -81.2 69.7 2(CH ) CO-5HC1 

-76.9 47.1 " -80.8 71.7 " 

-78.0 54-0 " -85.3 74.3 

-80 52.91 " 

Data for the reciprocal solubility of HCl (also of CCL, S0 2 and ML) 
and the vapors of Ether, Acetone, Methyl Alcohol and Chloroform, as deter- 
mined by measuring at 25 the change in pressure produced by adding weighed 
amounts of the volatile liquid to a given volume of HCl gas, are given by 
MacFarlane and Wright, 1934. 



577 
SOLUBILITY OP DRY HYDROGEN CHLORIDE IN SEVERAL SOLVENTS 

AT 20 AND 76omnK 
( 1^1 rbro then and Balltin, 1931.) 



HYDROGEN H 



Solvent Qua. HC1 per lOOOcc sat. solution 

Benzene (C 6 H fl I 16.91 

Carbon Tetrachloride (CC1 4 ) 6.19 

Cyclo Hexane (C fi H ) <^ 9q> ( I7 ~i8) 

Cyclo Hexene ?H g Cn g CH g CH g CH;yH) 12.29 (17-18.6) 

SOLUBILITY OF HYDROGEN CHLORIDE IN SEVERAL SOLVENTS AT 20 AND 76omm. 

(Dell, 1931.) 

The solvents were saturated by bubbling HC1 through them for about 3 
hours, using some 8-10 times as much gas as required for saturation. The 
dissolved gas was determined by displacing it with a current of CO free 
air and absorbing the fiCl in H ? and titrating it with normal NaOH. 



Solvent 


s 


X 


Solvent S 


X 


Hexane 


3-64 


0.0197 


Bromoform 4.78 


0.0306 


Octane 


4*50 


0.0296 


Ethyl bromide 10.3 


0.0348 


Dodecane 


3-42 


0.0314 


Chloroform 13.80 


0.0444 


Cetane 


2.28 


0.0270 


Bromobenzene 7.13 


0.0305 


Cyclo Ifexane 


342 


0.015^ 


Chlorobenzene 7.63 


0.0315 


Carbon tetrachloride 


4 -54 


0.0181 


Benzyl chloride 9.75 


0.0448 


Benzene 


11 .05 


0.0425 


Benzo tri chloride 4.77 


0.0275 


Toluene 


11 .90 


0.0507 


Tetra brom ethane^/ 3.93. 


0.0236 


Tetra chlor ethylene 


3- SB 


0.0163 


Tetra chlor ethane&6.20 


0.0265 


Tri chlor ethylene 


5-79 


0.0206 


Ethyl bromide 35i$ 


0.1019 


Penta chlor ethane 


3-86 


0.02lq 


Ethylene chloride 14.74' 


0.0457 



Cl 



S = the partition coefficient of IICl between the liauid and the vapor; 
that is s - C (the gm. eq.uiv. HC1 per liter) 4-0.0417, since s/c - 
22.4 x 293/273; x = the mole fraction solubility calculated on the assump- 
tion that the densities of the Solutions obey the ideal mixture law. 

One liter sat. solution of HCl in C H contains 3.13 am. HC1 at 20. 
(Knight and ifinshelwood, 1927.) 

One liter sat. solution of HCl in CIIC1 3 contains 1.83 am. HCl at 10. 
(Williams, 1921 . ) 

SOLUBILITY OP HYDROGEN CHLORIDE IN SEVERAL SOLVENTS. 

(Hamal. 1935.) 

A X7 shaped gas huret was used for absorbing the MCI in the several sol- 
vents. From the volume change in the gas buret, the initial and final 
pressures and the volume of the system, the volume of HCl actually absorbed 
at various pressures by the liquids was calculated. The results for 20cc 
volumes of solvent at the observed pressures were plotted and the value 
for 76omm pressure was found by extrapolation. The final results were 
calculated to Mol. fraction of HCl absorbed at 76omm. 



Solvent 



Formula 



Tetra Chlor Ethane C 2 H 2 C1 4 1.1.2.2 

Carbon Tetra Chloride CC1 4 

Ethylene Chloride 

Ethylene Bromide 

Tri chlor Ethane C 2 'H Cl .1.1.2 

Penta chlor Ethane CJifil 



C 2 I! 4 C1 2 



. 



b. pt. of Mol 


. Fraction HCl 


absorbed 


at 7eOmm at: 


solvent ' 


150 




20 




25 


2 143 


.5 





0. 


03006 


0. 


02744 


0. 


02481 


76 


.0 





0. 


01826 


0. 


01550 


0. 


01277 


83 


.0 





0. 


04377 


0. 


03993 


0. 


03576 


129 


.0 





0. 


03754 


0. 


03441 


0. 


03116 


'. 112 


5 





0. 


03463 


0. 


03101 







159 


.0 





0. 


02396 


0. 


02250 








H HYDROGEN 



578 



Freezing-point data are given for the following mixtures: 



HC1 + Chloroform 

" f Methyl Alcohol 

11 + Methyl Chloride 

11 + Methyl Ether 

" * Propionic Acid 

" + Hydrogen Sulfide 

11 * Magnesium Chloride 

11 + Sodium Chloride 

" + Sulfur Chloride 

" 4 Sulfur Dioxide 



(Baume and Borowski, 1914.) 

" " " " > Baume and Pamfil, 

1911, 191^ 5 Maass and Mclntosh, 1913.) 
(Baume and Tybociner, 1914.) 
(Maass and Mclntosh, 1912; Baume, 1911, 191*1..) 
(Baume and Georgitses, 1912, 



(Dernby, 1918. ) 

(Terrey and Spong, 1932.) 
(Baume and Pamfil, 1911, 1914.) 



PERCHLORIC ACID HC10 4 . 

SOLUBILITY IN WATER, (van Wyk/'igoa, 1905.) 

Mixtures of HCKX 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: 

Solid Phase. 
Ice 



HC10,. 3 iH 2 



Mols. HC10 4 
t. per 100 Mols. 
HClO 4 +HjO. 


O 


o 


10 


5 


21 


7 


-34-5 


9 


-54 


ii 


-50-5 


19 


-45 


20 


-42.3 


21 


-4I-4 


22.22 


-43 


23-5 


-40.5 


22.5 


-39-5 
-37^6 

-37-5 
-38-8 

-47-8 


22.7S 
24 
26 
27 
22.5 


~"44 


24 


-43-5 


*4-5 


-43.2 
-44-5 


25 
26 


-37.2 


25 i 



Hd0 4 .3H a O/9 



-32 
29.8 


Mols. HC10 4 

fdS+sfr Solidphasc - 

26 HC10 4 .2|H 2 
28.57 


-44 


27 


HC10 4 .2HjO 


-34 


27.25 
28 





-24 


29.9 


" 


17. 8m. 
-21.5 
-23.6 


^33-3 
36 
36.5 


" +HC10 4 .H*0 


-12.5 

+3 
28 


37 
38 
40.8 


HC10 4 .H,0 


40 


43-7 


tt 


50 m. pt 


So 


tt 


45 


59-9 





27-5 


71 .5 


M 


17 

+ 2.2 


77.2 
83-3 


M 
tt 


21.5 


90.7 


U 


-40 


94 


" 


IO2 


100 


' 



579 HYDROGEN H 

HYDROGEN FLUORIDE HP 

FREEZING-POINTS OP MIXTURES OF HYDROGEN FLUORIDE AND WATER. 

(C&dy and Hlldebrand, 1930.) 

The mixtures were contained in a gold cup provided with a gold plated 
stirrer. The temperatures were measured with a thermo couple encased in 
a platinum tube. To about loocc of solution in the gold cup enough liquid 
air was added to partially freeze the solution. After stirring for 15 
minutes the temperature was read and immediately afterwards a sample was 
removed for analysis. This was weighed in a paraffine lined bottle, 
diluted with water and titrated with NaOH using phenolphthaleine as indi- 
cator. In some cases it was necessary to determine warming curves and 
take the final sudden change in slope as the freezing-point. The authors 
give the observed freezing-points as K but in the following table they 
have been converted to the ordinary scale by deducting each one from -273. 

On. Mols. HF per Solid Q Gta. Hols. HF per Solid 

1 100 gn. Mols. HF+H 2 Phase l 100 PU Mola. HF * ti ? p Phase 

-0.9 0.777 Ice -75-4 69.8 2HF.H 2 

-6.3 5.6/1 

-9.8 8.09 

-23.0 15.65 

-41.4 21.6 

-60.0 26.5 

-70.1 27.6 

-62.7 30.7 

-59.4 32.1 

-48.9 37-1 

-43*5 40.3 

-36.1 47-8 " -106.9 89.4 HF 

-35-3 5o.o 

-35.8 51-5 

-41.5 57.5 

-51.0 62.7 

-68.3 67.5 

-75.1 68.5 

SOLUBILITY OF HYDROGEN FLUORIDE IN BBNZBNR. 

(Simons, 1331.) 

Vessels made entirely of copper were used. The vapor of HF at its b. 
pt . or that carried over by nitrogen from liquid HF maintained at other 
temperatures, was conducted into benzene until the saturation point was 
reached at selected temperatures. These results were plotted and the 
following values obtained from the curves. 

t of the Liquid HF from which On. Mols. HF dissolved per 100 gn. mola, HF 

Its vapor was conducted 

-77 

-18 



b. pt . 



Ice 


-75-4 


69.8 


M 


-75-7 


71 .0 


ti 


-81.7 


74-3 


" 


-91-1 


76.2 


" 


-101 .3 


77.6 


" 


-100.7 


78.6 


" + HF.H P 


-100.3 


79-6 


HF.H 


-100.2 


8o.O 


n 


-100.6 


81.7 


11 


-105.4 


86.4 


11 


-110.8 


88.3 


n 


-106.9 


89.4 


n 


-99.7 


91.3 


11 


"93.6 


93-9 


11 


-88.9 


96 .1 


11 


-86.9 


97.4 


11 


-85.4 


98.2 


" + aHF.H.O 


-82.9 


100.0 



30 


30 


40 


50 


60 ' 


2.48 


2.03 


1.58 


1 .12 


0.71 


3-85 


3.15 


2.44 


1-73 


1.02 


4.32 


3.55 


2.75 


1 .96 


1.17 


6.73 


5.48 


4-22 


2.98 


1.80 



Vapor pressure results are also given. 



H HYDROGEN 



580 



Similar determinations of the solubility of HP vapor at its b. pt. in 
octane, gave the following results. 

25-1 36.0 45.2 51.0 66.3 
0.338 0.276 0.235 0.194 0.170 



t of sat. sol. in Octane 



Mols. HP per 100 mols. HP * C H 

8 18 

Freezing-point data for mixtures of HP + KP are given by Cady, 1934, 
and the mixtures of HP 4 NH 3 by Ruff and Staub, 1933. 

HYDRIODIC ACID HI. 

SOLUBILITY IN WATER, DETERMINED BY FREEZING-POINT METHOD. 

(Pickering, i893a.) 
Cm. HI 

t. per 100 Gms. Solid Phase. t. 

Sat. Sol. 

Ice 60 



Cms. HI 

per 100 Cms. Solid Phase. 
Sat. Sol. 



10 

20 
-30 
-40 

50 

60 

-70 



20.3 

29.3 
35.1 
39 

42 

44.4 

46.2 
47.9 



+HI. 4 H 2 



40 

about-35.5m.pt. 
-40 

49 

48m.pt. 

-56 
5"2 



52.6 


HL 4 H 2 


59 


" 


64 


" 


65-5 


*( 


66.3 


" +HL 3 H 2 


?o-3 


HI 3 H 2 


73-5 


" H-HI.aHjO 


74 


HI aHjO 



F.-pt.dataforHI 4- H 2 S (Bagster, 1911), HI + (CH 3 ) 2 0. (Maass and Mclntosh, 19114 
HYDROGEN IODIDE 

EQUILIBRIUM IN THE SYSTEMS HYDROGEN IODIDR, WATER AND ALCOHOLS. 

(Rebum and Shearer, 1933.) 

The determinations were marie by adding from a buret one of the con- 
stituents to known mixtures of the other two,until appearance of a per- 
manent turbidity. The tie lines of the saturation curves thus obtained 
were determined by mixing suitable amounts of the three constituents to 
yield two liquid layers and titrating each of these for acid content. 

Results for HI 4 ILO 4 Iso Amyl Alcohol Results for III + HO 4 Iso 

UCH 3 ) 2 CHCH 2 CH ? OH) Butyl Alcohol ( (CH 3 ) g CIICH 8 OH-) 

Oms. per 100 jgns. sat, sol, ftna. per 100 gma. sat, sol. Qms. per 100 gns. aau sol. 

'-H- CO ^'H CH W ^ ^^ C 4 H 10 ^ 



8.50 


91-5 


12.0 


62.8 


21.0 


58.8 


24.. o 


52.6 


25.8 


47.5 


27.8 


43.2 


29.1 


40.1 



43-2 


15-7 


62.3 


2.76 


76.6 


2.55 


77-5 


3.03 


91.2 ~ 


2.98 


97.2 


2.80 



l6.1 
24.9 
32.0 
37.8 
39-6 
61.9 
91.2 



C 4 H 10 

83.9 
67.0 
54-7 
46.7 



19.3 
8.8l 



Tie Line Data 



Oms. HI per 100 gma.: 



H6layer 



30.0 
41.1 



9-45 
21.1 
30.5 



_ 
' H g O layer 

11.6 
4.8 



Tie Line Data 

Oms. KI per lOo gma.: _ 
layr x 



8.3 
4.0 



HYDROGEN H 



FREBZING-POINTS OP DILUTE AQUEOUS SOLUTIONS OP HYDROGEN IODIDB. 

(Klein and Svanberg, 1920.) 



1 Of F. pt. 

-0.35 
-0.91 
-1.90 



Normality of HI 

0.1 

0.25 

0.50 



OGEN IODATE HI0 3 

SOLUBILITY OF IODIC ACID IN 


WATER. 


(Groschuff, 1906.) 




t. G r 8 -' k? 3 ? 6 ^ Solid Phase. t. 
100 Gms. Sat. bol. 


Gms. I 2 Os per 
100 Gms. Sat. Sol. 


Solid Phase. 


o-3 


1.69 


Ice 


16 


71.7 


HIOj 


1. 01 


6.81 


" 


40 


73-7 


. 


2.38 


26.22 


" 


60 


75-9 


'' 


4.72 


51.42 


" 


80 


78.3 


tt 


6.32 


57.61 


" 


85 


78.7 


" 


12.25 


67.40 





IOI 


80.8 


" 


14 


69.10 


" +HIO, 


no 


82.1 


HI0 3 +HI 3 O 


15 


70 


(unstable) Ice 


125 


82.7 


HlaOg 


19 


72 


" 


140 


83-8 


" 


o 


70^3 


HIO 3 


160 


85-9 


it 


SOLUBILITY OF IODIC ACID IN 


NITRIC 


ACID. (Groschuff.) 




Gms. HI0 3 per 100 Gms. 




t. 


Aq. 27-73 


% HN0 3 


40.88% HN0 3 








Solution. Sc 


jlution. 


Solution. 






o 


74 I 


18 


9 






20 


75-8 


21 


10 






40 


77-7 


27 


14 






60 


80 


38 


18 





10 



SOLUBILITY OP HYDROGEN IODATB IN AQUEOUS SOLUTIONS OF 
NITRIC ACID AT 25. 

(Moles and Perez- VI torU, 1931. 1932.) 



Wt. Percent 



20.23 
28.00 
35.28 
43.32 



d of the 

HN0 3 HgO 

mixture 

1.123 
1.173 
1.223 
1.273 



Otos. HICLper 100 Wt. Percent 
HNO, 



gms. sat. sol. 

35-09 
21.8^ 

15.20 
10.08 



50.71 
58.66 
65.30 



dof the 

HNO^ * H 

mixture 

1.324 
1.366 
1 .400 



Ons. HI0 3 per 100 
gns. sat. eol. 

5.7^ 
3-25 



H HYDROGEN s82 

HYDROGEN NITRATE (Nitric Acid) HN0 8 

RECIPROCAL SOLUBILITY OF NITRIC ACID AND WATER, DETERMINED BY THE 
FREEZING-POINT METHOD. 

(Kiister and Kremann, 1904; see also Pickering, 1893.) 



*- 

10 
~2O 



Cms. HN0 3 

per 100 Gms. 

Sat. Sol. 



Solid Phase. 



13-9 
22.9 
2 7 .8 

3 J -5 

32-7 

34-1 

40 

49.2 

53-8 

58.S 

65-4 



Ice 



HN0 3 . 3 H 2 



t*. 


Gms. HN0 3 
per 100 Gms. Solid Phase. 




Sat. Sol. 




-40 


69.7 


HN0 3 .3H 2 


42 Eutec. 


70-5 


" +HN0 3 .H 


-40 


72-S 


HN0 3 .H 2 


-38 m. pt. 


77-75 


" 


40 


82.4 


" 


50 


86.5 


" 


-60 


88.8 


" 


66.3 Eutec. 


89-95 


" +HN0 3 


-60 


91 .9 


HN0 3 


-5o 


94.8 


" 


~4i.2m.pt. 


100 






-40 

43 Eutec. 

-40 

-30 

20 

18.5 m. pt. 

20 
- 3 o 

NITRIC ACID. 

FREEZING-POINTS OF AQUEOUS NITRIC ACID SOLUTIONS. 

( Klein and Svanberg, 1920. ) 

Normality of Normality of 

t - of f. pt. uq. HNO a . t of f. pt. aq. HN0 3 . 

0.885 0.^5 1-797 o.5o 

OF NITRIC ACID AND NITROGEN PEROXIDE (N 8 4 ). 
( Pascal and Gamier, 1919. ) 

Thermic analysis was used for determination of the solubility at very low tempe- 
ratures and for the detection of the internal transformations in the system. 

Solubility, in the Liquid State, of : 
NjiQv in HNO 3 . HN0 3 in N 2 O 4 . 



t" o 



Normality of 
a<I- HNO S . 

0.356 ...... o.io 

RECIPROCAL SOLUBILITY 



t". 



Gms. HNOj per 
100 gras. mixture. 



Solid 
Phase. 



-42 ....... ioo. o HNO 3 



-58.5 
-70 



-58.5. 
-48.5 
-32... 
-21.4. 



90.6 

85 

82 

70 

66 

62 

60 



ftOt (Solid) 

(solid) 





Gms. HNO S per 


Cms. IIX0 3 per 


t, 


100 gms. mlxlu'rc. t". 


100 gins, mixture. 


II . 


... 52. o -i3.25.. 


... 2.75 


- 0.8. . 


. . 5o - 5.o. . . 


... 4 2 


-u5 


45 + 5.0. . . 


5 . 20 


20 .... 


... 44.3 ig.5... 


7.i5 


35 


3?. 5 4o.o... 


. . IO.O 


5o.... 


... 3o 55.o... 


... 20.0 



Determinations of the compositions of the two liquid layers which are formed 
in the system nitric acid and nitrogen peroxide at certain temperatures, were made 
by Bousfield, 1919, by means of density measurements, and the following results 
were obtained. 



N,0 4 inHNO 





Density 


Specific 


Per ceni 




t ft . 


of mixture. 


volume. 


11X0,. 


t. 


4-0... 


1.65432 


o. 6o448 


45.6 


4.0... 


II. O. . . 


1.63942 


0.60997 


45.7 


ii .0. . . 


18.0... 


1.62601 


0.6l538 


46.o 


18.0... 



HN0 3 in N 2 5 . 

Density Specific Percent 

of mixture. volume, TEX0 3 . 

1.48742 0.67231 4-90 

i.4735i 0.67865 6.67 
1.45940 0.68521 8.o5 



5*3 HYDROGEN H 

Freezing-points of mixtures of HN0 3 + H g S0 4 + H ? over a wide range of 
composition, especially for the region of high concentration of H 2 SO , 
have been determined by Holmes, 1920, Carpenter and Lehrman, 1925 and 
Holmes, Hutchinson and Zieber, 1931. These latter investigators give a 
triangular diagram constructed from all available data on this system, 
showing the iso thermal freezing curves for mixtures of varying percen- 
tage composition . 



NITRIC ACID HNO S . 

DISTRIBUTION OF NITRIC ACID BETWEEN WATER AND ETHER AT 25. 

(Bogdan, 1905, 1906.) 

Mols. HNO n Per Liter of: Mols. HNO :) per Liter of: 

/ * \ t *> -% 

H 2 Layer. Ether Layer. H 2 Layer. Ether Layer. 

0.9145 0.0855 0.09005 O.OOlSl 

0.4811 0.0278 0.04749 0.00064 

0.2644 0.00894 0.02760 O.OOO29 

0.1392 0.00278 0.02462 0.00025 



Data for the distribution of HNQ, between Water and each of the fol- 
lowing compounds; Ether, n Butyl Alcohol, n Amyl Alcohol and Methyl 
Ethyl Ketone are given by Archibald, 1932. 

HYDROGEN OXIDE (Vfater) H ? 

Note - Data for the Reciprocal Solubility of Water in Organic Solvents, 
in addition to t hole here shown, will be found in Volume 2., under the 
respective Organic Compounds. 

RECIPROCAL SOLUBILITY OF WATER AND SEVERAL ORGANIC COMPOUNDS AT 20. 

(Evans. 1936.) 

The author describes an improvement of the Hill, 1923, method of deter- 
mining the mutual solubility of liquids, which consists in the more suit- 
able choice of the volume ratios of the two liquids. He also describes a 
simplified form of apparatus to be used. 

The following results were obtained with the improved technique. 

Solvent, Water Solvent, Organic Compound 

d 20 Qf a" 3 - O r *. Solvent d SQ of 

Organic Solvent satJsol. PCr ^ aw* sol. 10 * 8 ' 

sac. sol. in H^p In Org. Solvent 

Sec. Butyl Alcohol 0.971 18.5 0.880 64.4 

Methyl Ethyl Ketone 0.962 26.7 0.836 87.9 

Methyl tert. Butyl Ether 0.990 4.8 0.745 98.5 

Methyl tert. Amyl Ether 0.995 ^-25 0.771 99-3 

Chloroform 1.001 0.8 1.486 99.8 



HYDROGEN 584 

SOLUBILITY OF WATER IN SEVERAL ORGANIC SOLVENTS. (Clifford, 1921.) 
The saturated solutions were analyzed by volatilizing the sample and absorbing 
the moisture in a dehydrating agent (Ca C1 2 ) which does not absorb or react with 
the organic solvent. 

Gms. Ha per Gms. II., per 

Solvent. t. 100 gms. sat. sol. Solvent. t- uu) gms. "sal. sol. 

Benzene ....... 21.0 o.o46 Carbon disulfide ?.5.o o.oio 

26.6 o.o56 9.6. o o.oi i 

42 . 088 27.O O . O I'). 

55. o o.n3 Carbon tetracbloride. 24.0 o.oio 

Chloroform 24-5 0.084 28.5 o.oi.'i 

.... 26.7 0.107 Gasoline.. 26.0 o.oo85-o.oioo 

.... 27.8 0.116 . 35. o 0.0121-0.0161 

37.5 0.0145-0.0175 

Results for the Solubility of H 2 0, Blood and Oils in cycle Propane 
((pH 2 -.CH g .pH g ) are given by Orcutt and Seevers, 1937. 

SOLTIBILITT OP WATER IN BBNZINB, TOLUBNB AND CARBON TBTRACHLORIDB . 
(Hosenbaura and Walton, 1930.) 

TThe H 2 dissolved in the organic solvents was determined by converting 
it to HgWith the aid of calcium hydride according to the reaction 2lI 2 -*- 
CaHg = Ca(OH) 2 * 2H 2 . Very high accuracy is claimed for the method, but 
it cannot be employed with solvents which react with Call 2 and the deter- 
minations require considerable time for completion of the reaction. 

Qns. H.O dissolved per 100 gms. 



10 
20 
30 
40 
50 
60 

The presence of CS e in CCl^ as an impurity was found to increase the 
solubility of water in this solvent about 50 percent. 

SOLUBILITY OF WATBR IN BBNZBNB, TOLUBNB AND CYCLO UBXANB, 

(Tarassenlcow and Poloshlnzewa, 1931. 1932.) 

The determinations were made by the synthetic method of Alexieff as 
improved by Rothmund. 

Results for C e H 6 Results for C fi H 5 CH 3 Results for C fl H lg 



Ve 


VB^S 


cci 4 


0.0451 

0.0573 
0.0746 


0.0335 
0.0450 
0.0600 


0.00711 

0.00844 

0.0109 


0.0953 


0.0733 


0.0152 


0.1271 
0.1637 


0.0953 


0.0237 



Q 


(fas. H per 




ns. HgO per 


,0 


Ghis. HgO per 




100 8*s. sat. sol. 


C 100 1 


ajna. sat. sol. 


t 


100 gnts. sat. sol. 


5.0 


0.024 


-9.0 


0.002 


14.0 


0.005 


9-5 


0.034 


-3.5 


0.005 


19.0 


0.010 




0.041 


+10.5 


0.020 


28.5 


0.015 


22.5 


0.060 


18.0 


0.034 


32.5 


0.020 


32.0 


0.082 


30.0 


0.053 


38.0 


0.031 




0. 102 


48.0 


0.097 


53-0 


0.050 


56* 


O.l8l 


60.5 


0.153 






67.5 


0.251 


76.0 


0.254 







73.0 0.300 930 0.413 



HYDROGEN OXIDE (Water, 5 * 5 HYDROGEN 

SOLUBILITY OF WATER IN BENZENE. (Hill, 1923.) 

A new thermostatic method was employed. This is based upon the unusual 
solubility relations of silver perchlorate. This compound is soluble in various 
organic solvents and exceptionaly soluble in water. Consequently, the presence 
of small amount) of water in an organic solvent greatly increases the solubility 
of silver perchlorate in that solvent. The method consists in making a reference 
curve for the solubility of silver perchlorate in the organic solvent containing 
known amounts of water. Saturated solutions of water in the organic solvent 
arc then made at various temperatures and each of these used as solvent for silver 
perchlorate at the temperature of the reference curve. By comparison with the 
reference curve the percentage of water in the solvent becomes known. The data 
for the reference curve of silver perchlorate in benzene + water mixtures afe 25 
will be found under silver perchlorate at the bottom of page 1401. The estimated 
results for the solubility of water in benzene are as follows. 

Gms. TIjO per io<> Gins. II 4 per 100 Gms. 1LO per 100 

t". gms. sat. solution. t". gms. sal. solution. t". gms. sal. solution. 

S.o ...... o.o35 37.5 ...... 0.109 65. o ...... 0.23-2 

f>.4 *.. 0.037 4^.0 ...... 0.118 66. o ...... 0.^38 

i5.o. ..... o.o5i 5o.o...... o.i58 69.5 ...... o.-2;58 

j3.o ...... o.o(>' 5:5.o ...... 0.181 77 .o ...... o.3(>4 



Data for the effect of HO upon the Critical Solution Temperatures of 
mixtures of CH^Oii + CS 2 , CH^OH + a Hexane and CH OH + Cyclo Hexane are 
given by rte Brouckere and (Jillet, 1935. The autnors used the results 
as the basis of a method for the determination of H 2 0. 

SOLUBILITY OF WATER IN BENZENE SOLUTIONS OP MONO, Di, AND 
TRI CHLOR ACETIC ACIDS AT 15 

(Bell, 1930.) 

Results for solutions in C-H> of: 

O 



v_ 


HgClCOOH 


CHClgCOOH 


CC1 3 COOII 


On. Hols. 


per 


On. Mols. 


per 


On. Hols, per 


d of 


1000 gms. 


sat 


. sol. 




n of 


1000 m*^ 


.sa 


t. sol. 


d of 


1000 . 

, /N 


sac. sol. 


sac. sol. 


CHgClCOOH 


., .. 3t. SOJ. 


CHClgCOOH 




H 2 


sat. sol. 


'CHjClCOOH 


H/"^ 


0.884 


0.0620 


0. 


0329 





.880 


0.035 





.0408 


0.878 


0.0278 


0.0426 


0.88l 


0.115 


0. 


0423 





.880 


0,071 





055 


0.878 


0.0506 


0.0690 


0.880 


0.174 


0. 


0574 





.883 


o. 123 





.101 


0.887 


0.0950 


0.115 


6.885 


0.217 


0. 


0045 





.895 


0.179 





.130 


0.885 


0.140 


0.165 


0.888 


0.284 


0. 


0776 





.890 


0.195 





.138 


0.888 


o. 176 


0.210 


0.886 


0.325 


0. 


08P-8 












0.892 


0.219 


0.247 



0.892 0.404 0.1 000 

The author recalculated the results of Waddell, 1898, for benzene solu- 
tions of acetic acid at 25 and obtained the following values. 

dor O. Mols. per 1000 gna, sat. sol. 

sar,. sol. ' CH~COOH ' H^O ^ 

0.874 0.077 0.011 

O.876 0.2 IS 0.0? 1 



H HYDROGEN 5*6 



SOLUBILITY OP WATER IN BENZENE, TOLUENE AND XYLENE 
SOLUTIONS op ETHANOLAMINE OLEATE (SOAP) 
(Pint, 1938J 



Gkn. Hols. Ettianolamlne 


cc H/jO dissolved per SOcc of Ethanolawlne Solution in 


Oleate per liter 
organic solvent 


'Benzene (CgHg) Toluene fCgHj-CH^) 


Xylene C 6 H 4 (CH 3 ) ? ; 


0.05 


O.l8 


0.17 


O.l8 


0.10 


0.38 


0-34 


0.36 


0.20 


0.70 


0.68 


0.69 


0.30 


1.06 


1.0$ 


1.08 


0.40 


1.40 


1.32 


1.36 


0.50 


1.70 


1.68 


1.68 


0.60 


2.08 


2.03 


2.07 


0.70 


2.35 


2.34 


2.36 



The determinations were made by adding the water from a microburet 
to the mixtures until on active shaking a faint cloudiness appeared. 
The temperature is not stated but was probably that of the room. The 
quantity of water dissolved is proportional to the quantity of the 
Ethanolamine oleate (soap) present. It was also found" that additions 
of small quantities of phenol greatly increased the amount of water 
dissolved. Further quantities of phenol however caused the solutions 
to become cloudy again. 



SOLUBILITY OF WATER IN BENZENE, PETROLEUM AND PARAFFINE OIL. 

(Groschuff, 1911.) 

The synthetic, sealed tube method was used and the experiments were made 
with very great care. The mixtures were first superheated sufficiently to bring 
all the water into solution and then cooled until a fine mist was formed. The 
temperature of appearance and disappearance of this fine mist was determined re- 
peatedly. The benzene was of <4> = 0.8799. The petroleum was American 
water white, of d = 0.792. It was freed from H^O 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 dis = 0.883 and b.-pt. was 2OO-3OO at 10 mm. 
pressure. 

Results for: 

H 2 O -f Benzene. H 2 4* Petroleum. H 2 O + Paraffine Oil. 



t o Gms. H 2 
' per TOO Gms. Sol 


t o Gms. H 2 
per 100 Gms. Sol 


t o Gms. H 2 ,o Gms. H 2 
* per 100 Gms. Sol. * ' per 100 Gms. Sol. 


+ 3 


0.030 


2 


O.OOI2 


59 


0.031 


+ 16 


0.003 


23 


0.061 


+ 18 


O.OO5 


61 


0-035 


So 


0.013 


40 


0.114 


23 


O.OO7 


66 


0.043 


65 


O.O22 


55 


0.184 


30 


O.OOS 


79 


0.063 


73 


0.030 


66 


0.255 


36 


O.OI2 


85 


0.075 


77 


0-035 


77 


o-337 


53 


O.O26 


94 


0.097 


94 


0-055 



Observations on the solubility of water in essential oils are given by Urnney and 
Bunker (1912). 



587 HYDROGEN H 



HYDROGEN OXIDE (Water) 



SOLUBILITY OF WATER IN AVIATION GASOLINES. 

(Aldrlch, 1931.) 

The samples of gasoline were saturated with H ? by shaking the mixture 
in an evacuated bulb, provided with all the refinements for accurate 
removal of the saturated sample for analysis. The H in this sample 
was determined by adding sodium-potassium alloy, free of oxide, and 
collecting and measuring the evolved hydrogen. The determinations were 
made with the greatest possible accuracy. 

Q 0. H g O per 100 0ns. sat. solution in Gasoline No.: 

t / ~ io 12 13' fS 19 s 

10 0.0128 0.0051 0.0071 0.0055 0.0036 

30 0.0160 0.0067 0.0086 0.0172 0.0052 

50 0.0193 O.OO79 0.0101 0.0208 0.0069 

Gasoline sample No. 10 - Oklahoma natural gasoline, d lg = 0.677. 

11 " No. 12 = West Virginia natural gasoline, d lg - 0.695. 

" " No. 13 = California Crude, d lg = 0.695. 

" " No. 15 = Midcontinental crude, d lg = 0.718. 

11 " No. 19 = Oklahoma natural gasoline, d is = 0.682. 



Except for fuel No. 15 the change in solubility with temperature is 
represented by a straight line 

Using the calcium chloride method, Clifford, 1921, obtained the fol- 
lowing values for the solubility of H ? in gasoline of d - 0.700 

pis. sat. solution 

25 0.0085; 0.0110 

35 0.0l6i; 0.0121 

37-5 0.0175; 0.010-5 

The Army Air Corps, 1922, using the calcium chloride method found 
the solubility of water in domestic aviation gasoline at 23.9 to he 
0.007 g m - ^2^ P er 10 ms * sa -t. solution. 

Using the same method Uspenskii, 1929 obtained the following results: 

Cta. H 7 jper 100 ma. sat. sol. at: 
Gasoline *- ~ ^ , 

Grozny "avis" 0.007 0.011 

" grade I 0.006 0.008 

11 grade II 0.006 0.008 

Baku grade II 0.005 0.008 



H HYDROGEN 

HYDROGEN OXIDE 



(Water) 



588 



WATER TOLBRANCE OF MIXTURES OF GASOLINE WITH ETHYL ALCOHOL 
Iso PROPYL ALCOHOL AND BENZENE. 

(3ayiey and Hopkins, 1934.) 

The mixtures contained in a test tube provided with a thermometer and 
a stirrer were cooled in a Dewar flask containing acetone and CCL snow 
until the cloud point was reached. The tube was then removed and the 
point at which the cloud just disappeared with rising temperature, was 
taken as the critical solution temperature. Three samples of gasoline, 
two of Iso propyl Alcohol and a series of samples of Ethyl Alcohol con- 
taining from 1.63 to 5.65 Volume percent ll ? Q were used. Numerous dia- 
grams showing the observed c.s.t. of various mixtures of the gasolines, 
alcohols and water are given. From these, various tables are constructed 
which show the relation of HO content to c.s.t. in mixtures of varying 
composition. Thus, for example, the critical Water Content of Mixtures 
containing 90, 80 and 70 percent of regular grade automobile fuel 
(liquid phase cracked gasoline) is as follows. 



Vol. Percent 



Compofll 



ilUon of Mixture 



asollne 


Ethyl Alcohol 


Iso propyl Alcohol" 


90 


10 





90 


8 


2 


90 


7 


3 


90 


6 


4 


80 


20 





80 


16 


4 


80 


12 


8 


70 


30 





70 


25 


5 


70 


20 


10 



Critical H. 


gO Content In Vol. 


* at: 


> 6~ 


-20 


-40 ' 


0.30 


0.22 


0.15 


0.35 
0.38 


0.27 
0.30 


0.19 
0.22 


0.41 


0.33 


0.25 


0.70 


0.50 
0.64 
0.80 


0.35 
0.46 
0.6o 


1.25 


0.84 
1 .09 


0.59 
0.76 





1.25 


1 .00 



Iso propyl Alcohol increases the water tolerance and the critical 
water content of any ethyl alcohol-gasoline mixture to which it is 
added. Benzene may be used to increase moderately the critical water 
content of ethyl alcohol-gasoline mixtures by substituting benzene for 
part of the gasoline. Its effect, ttowever, in increasing water toler- 
ance appears to be too slight to be of practical value. 

HYDROGEN PEROXIDE H,0,. 

FREEZING-POINTS OF MIXTURES OF HYDROGEN PEROXIDE AND WATER. 

( Maass and Herzberg, 1920. ) 



t f Urns If*0 4 per 
r. pt. loo gins, mlxliin 


Solid 
Phase. 


t of Cms H,0. per Solid 
f. pt. 100 gms. mixture. Phase. 


2.O... 


100 


H,0 2 


5 I .7 


49.8 H 2 2 .2l: 


i4o . . . 


86.0 





1)0.8.... 


47 o 


22.7... 


80.45 





5 1 . 8 .... 


46 . 2 i 


36.5 ... 


74.0 





46.25 ... 


42.02 HjO 


39.5 . . . 


69.2 





-38.o.... 


37.80 


-.15.5 ... 


65.4 





35 .7 .... 


36.47 


56.O . . . 


63.o5 





-28.5.... 


31.96 


-52.5... 


61.14 


)) 


23.4 


27.72 


-54.5 ... 


58.8 


H a O,.2H,0 


17.0 


22 . 5O 


-54.3... 


56.2 





ii .1 .... 


15.91 


-53.6... 


55.o6 





6.3.... 


9.96 


-02.5 ... 


53.7 





- 3.4.... 


4-9 



HYDROGEN 



HYDROGEN PEROXIDE HgO^. 

EQUILIBRIUM IN THE SYSTEM HYDROGEN PEROXIDE, UREA AND WATER. 



To aqueous hydrogen peroxide solutions of known concentrations 
weighed amounts of urea were added and the mixtures warmed until clear. 
Upon cooling the temperature was determined at which crystals separated. 
The Solid Phases were ice, urea or the double compound CO(NH 2 1g.H 2 2 . 



Temp, of Saturation of Solution containing* 



In Aqueous 


10 Wt, 


<* 


20 Wt.* 


30 Wt. 


% 


40 Wt 


. % 


50 Wt. % 


60 Wt. 


% ^ 


Solvent 


CO(NH 2 ) ? 


CO(NH 2 ) g 


CO(NH ? ) 


2 


CO(NH g ) 2 


CO(NHg) 2 CO(NH 2 ) 2 


3-0 


-5- 





-6.5 


-9.7 




-0.8 




+16. 


5 


+35. 





6.0 


-6. 





-7.5 


-2,0 




+6.0 




+ 12. 


2 


+20. 


3 


10. 


-8. 





-2.0 


+30 




+5-5 




+ 14 . 





+34- 


5 


15.0 


-3. 





+6.0 


+ 11.6 




+13.5 




+ 15- 


2 


+32. 


o 


20.0 


+2. 


7 


+ 12.2 


+ 19.2 




+21.0 




+22. 


5 


+ 31 . 


5 


30.0 


+7. 





+ 20.3 


+27.5 




+32.0 




+34- 


5 


+34- 


* 


Wt % H ? 2 


Temp, of Saturation of Solution containing: 


In Aqueous 


/ 5 Wt 


. * 


10 Wt. % 


15 Wt. 


% 


20 Wt. 


% 


25 Wt. 


, * 


33.7 Wt. 


% 43.7 Wt.% 


Solvent 


CO(NH 


?>2 


CO(NH 2 ) 2 


CO(NH 2 ; 


>* 


CO^ 


!>B 


CO(NHj 


2 ) 2 CO(NH 2 ) 2 CO(NH g ) 2 


30.0 


-1 


.0 


+ 12.0 


+20. 





+25. 





+30. 


5 


+ 36.0 


"**tiO . 5 


47.7 





.0 


+ 15-0 


+25. 





+31. 





+ 3 8. 











59.9 


+2 


.0 


+ 11.0 


+22. 


5 


+33- 
















79.1 


-tt 


.0 


+ 12.5 


*-26. 


o 


+35- 


5 


+47. 


5 








91.8 


-20 


.0 


+4-0 


+20. 





+31. 


5 


+4$. 












FREEZING-POINTS op MIXTURES OF HYDROGEN PEROXIDE AND METHYL ALCOHOL. 

(Matheson and Maass, 1929.) 

Om. Mol. CHgOH On. Mol. CH OH 

r o per 100 0n. mols. S 11(1 r o per 100 9. mols. Solid 

Pha3C C CH 3 OH4H 2 2 "*" 

-1.7 5.6 H 2 P -18.6 28.3 H 2 g 

-6.q. 13.2 " -22.2 33.2 " 

-10.2 18. i\. " -37.8 43-8 " 

-15.3 25.2 " -49-3 51.5 " 

The authors also give results for the freezing-points of mixtures of 

hydrogen peroxide and each of the following compounds: Ethyl Rther, 
Piperidine, Di ethyl amine, Mono n Butylamine, Tertiary mono Butylamine, 
Di iso Butylamine, Tripropylamine and Oi methyl amine. 



H HYDROGEN 



DISTRIBUTION OF HYDROGEN PEROXIDE BETWEEN WATER AND ETHYL ETHER 
AT 18. (cle Kolossovsky, 1919, 1925.) 

The mixtures of equal volumes of water and ether, to which different amounts 
of redistilled Perhydrol were added, were vigorously shaken during. 20 minutes, 
by periods of 2 minutes each, and allowed to stand in the thermostat between the 
agitations and for I hour after the last. Aliquot portions of each layer were titrated 
with aqueous K Mn 4 solution in presence of sulfuric acid. The determinations 
were plotted and the following results were obtained from the curve. 



Cms. H S S 


per 100 cc. 


p. 


Cms. II S S per 


100 CC. 


P m 


II 2 laycr"5" ( 


c7H s )g6 layer (pS- 


Pi 


H S layer "). (C S H S 


Co layer (p\)] 


P^ 


0. 9 35 


O.O65 


14.4 


17.908 


2.092 


8.6 


2.795 


0.205 


i3.6 


19,. 590 


2.4lO 


8.1 


4.640 


o.36o 


12.9 


2 1 . 25 1 


2.749 


7-7 


6.470 


o.53o 


12.2 


23.7O7 


3.293 


7.2 


9-18-2 


0.818 


II. 2 


25.324 


3.676 


6.9 


10.968 


uo34 


10.6 


26.929 


4.071 


6.6 


12.734 


1.266 


IO. I 


28.522 


4.478 


6.4 


14-479 


1. 52 1 


9.5 


30.119 


4.881 


6.2 


16.204 


1.796 


9.0 


3i. 7 i4 


5.286 


6.0 



DISTRIBUTION OF HYDROGEN PEROXIDE BETWEEN WATER AND ORGANIC SOLVENTS. 

(Walton and Lewis, 1916.) 

Different amounts of perhydrol (30% H 2 O 2 solution) were added to various 
mixtures of water and organic solvents and, after constant agitation for about 
I hour, the H 2 02 in each layer was determined. 



Solvent 

Ethyl Acetate 
Isobutyl Alcohol 
Amyl Acetate 
Acetophenone 
Ether 
Ether 
Aniline 


t. 

25 
25 
25 
25 
2$ 



25 


Ratio, 
Cone. aq . 


Solvent. 

Methyl Iodide 
m Toluidine 
Phenol 

Quinoline 
ti 

it 


t. 

25 
25 
25 
o 

25 
40 


Ratio, 
Cone. aq. 


Cone. ojg. solvent 
3.92- 4. II 
2.58- 2.63 
13 -13-2 
5.82- 6.06 
8.28- 9.II 

5-72- 5.85 
4.08- 4.IO 


Cone. ortf. solvent 

Approx. 200 
Approx. 5 

4-35 -5-55 
0.276-0.391 
0.365-0.642 
0.516-0.602 



The following approximate values, determined at room temp., are quoted from 
the dissertation of A. Braun, Univ., Wisconsin, 1914. 



Solvent. 



Ratio, 
Cone. aq. 



Ratio, 



Solvent. 



Cone. a 



Solvent. 



Ratio, 
Cone. aq. 



Cone. org , solvent Cone. org. solvent Cone. O rg. solvent 

Ethyl Acetate Ethylisovalerianate -fa Isobutyl Alcohol J 
Nitrobenzene ^ Isoamyl Propionate ^ Propyl Formate i 
Acetophenone J Chloroform T } 7 Isobutyl Butyrate ^ 

Amyl Acetate J Benzene jfo Propyl Butyrate & 

The distribution ratio of hydrogen peroxide between water and ether at 17.5 
varies with concentration from 13.9 to 17.4. (Osipoff and Popoff, 1903.) 



59i HYDROGEN H 

DISTRIBUTION OF HYDROGEN PEROXIDE BETWEEN WATER AND AMYL ALCOHOL 

AT AND AT 25. 
(Calvert, 1901; Joyner, 1912.) 



Results at O. (Calvert, Joyner.) 

Mols. H 2 O? per Liter. pp 

^ _ .-_. 



Results at 25. (Calvert.) 
Mols. H 2 (\ ncr Liter. 



H 2 layer (W). Alcohol Layer (A). 



0.146 
O.2OO 
0.407 
0.749 
1.970 



0.0216 
0.030 

0.061 
0.113 
0.293 



6.76 
6.66 
6.63 
6.66 
6.71 



0.013 
0.028 



H 2 O Layer (W). Alcohol Layer (A). 
0.094 
0.194 

0.297 O.O42 

0.670 0.095 

0.913 0.130 



W 

A ' 

7.01 
6.91 
7.08 
7.09 
7.01 



Data are also given for the distribution of hydrogen peroxide between aqueous 
sodium hydroxide solutions and amyl alcohol at o and at 25. 

The following results for the distribution of hydrogen peroxide between 
water and Iso amyl alcohol lb.pt. 128- 130) at o are given by Ilusain, 
1927 1 but the terms in which the concentrations are expressed are not 
stated. 



Cone, of H g 2 in H^OfW) 

26.90 

32.12 



ln Alcohol (A) 



4.10 
4-93 



6.56 
6.53 







This author also gives results for the distribution of H 2 between 
Iso Amyl alcohol and aqueous solutions of sodium and potassium phosphates 
at o. 

DISTRIBUTION OF HYDROGEN PEROXIDE BETWEEN WATER AND AMYL ALCOHOL 

AT 0. (Mcn/el, 1923.) 

Gc. o.oon Thiosulfate solution Cc. o.oSn Thiosulfate solution 

required for 10 cc. of 
Aq. layer"!""!). AlcoholicTayer (A)? 

32.o5 4 60 

36. 5o 5.27 

43.83 6.36 

46. 5o 6.70 

52.85 7.73 

Data arc also given for the distribution of hydrogen peroxide between aqueous 
solutions of potassium metaboratc and tetraboratc, and amyl alcohol at o. 

Freezing-point Data have been determined for Mixtures of : 
H-CL + KC1 (Matheson and Maass, 1929-) 

II ^ V QQ ll II It II 

N Jp 4 



\v 


required 


Tor lOcc. of 


W" 


A 


Aq. layer iNVi. 


Alcoholic laycr(A) 


A 


6-97 


5*. 96 


7.70 


6.88 


6.96 


59.1 5 


8.6(> 


6.88 


6,89 


68 . oo 


io.o5 


6.80 


6.94 


76.2;) 


I I . 2,3 


<>-79 


6.85 









* , 
+ NaCl 
+ NaNO, 



(Maass and Hatcher, 1922.) 



HYDROGEN PHOSPHIDE (Phosphine) H 3 P 

One liter of Cyclo iiexanol (C fl H 1 jDH>lissolvei2.856cc H g P at 26 and 
766mm, Hg pressure. ((Cauquil, 1927.) 



H HYDROGEN 



592 



HYDROGEN PHOSPHITE (Phosphorus Acid) H^PQj 

Freezing-point data are given by Redfield and King, 1936, for each of 
the following mixtures. 



H PO, + CH.COOH (Acetic acid) 

'" + CCI 3 COOIi (Trichlor Acetic Acid) 

" + CH 3 COCOOH (Pyruvic acid) 

" * C 6 H 5 COOH (Phenol) 



(TH.COCII, (Acetophenone) 



C 8 H S C 



,) S fl H s CNO (Piperonal) 
IrCH.OCO (Co'imarin) 



PO 



HYDROGEN PHOSPHATE (Phosphoric Acid) 

PHOSPHORIC ACID (ortho) H 3 P0 4 . 

SOLUBILITY IN WATER. (Smith and Menzies, 1909.) 



(The sat. solutions 


were analyzed by 


tit rat ion. 


The mixtures were conste 


stirred for at least two hours.) 


Gms.H,P0 4 






Gms. HiPO 4 




t. per 100 Gms. 


Solid Phase. 


t. 


per zoo Gms. 


Solid Phase. 


Sat. Sol. 






Sat. Sol. 




-81* 62.9 


Ice-f2H,P0 4 .H 2 O 


24-38 


94.80 


ioH|P0 4 .HaO 


-16.3 76.7 2 


UPCVHjO 


24.40 


94.84 


" 


+ 0.5 78.7 


" 


24.81 


94-95 


* 


14.95 81.7 


" 


25-41 


95.26 


" 


24.03 85.7 


" 


25-85 


95-54 


" 


27 87.7 


" 


26.2* 




tt i TT 


29.15 90.5 


" 


26.23 


95.90 


H 8 P0 4 


29.35! 91.6 


" 


27.02 


95-98 





28.5 92.5 


" 


29.42 


96.15 


c 


27 93-4 


" 


29.77 


96.11 


" 


25.4 94.1 


" 


37-65 


97.80 


" 


23-5* 


" +ioH,P0 4 .H s O 


39-35 


98.48 





24.11 94.78 


ioH 3 P0 4 .H 8 O 


42-3of 


IOO 


" 




* Eutec. 


t M. 


P t. 





NOTE. The results of Giran (1908), determined by the freezing-point method, 
are shown to be erroneous, due to supercooling which would result from failure to 
induce crystallization by inoculation. 

F.-pt. data for mixtures of phosphoric and phosphorus acids are given by Rosen- 
heim, Stadler and Jakobsohn (1906). 



593 



HYDROGEN II 



SOLUBILITY OF ORTHO PHOSPHORIC Acm IN WATER. (Ross and Jonos, 1925.) 
The mixtures were stirred at constant temperature for at least three days. The 
analysis was made by titrating with standard Na OH solution, using phenolphthalein 
as indicator. 





Gms. H 3 P0 4 




[XT 1 00 gms. 


t". 


sal. sol. 


85 .K.iuf. 


:.. 6^.5 


57 , 


67, o 


13 


70 o 


2Q.O 


72 5 


17.5 


75 


o.o 


78.75 


18.92.. 


... 84.07 


23.41.. 


. .. 85.93 


25.24.. 


. .. 87.05 


27.30.. 


... 88.5i 


28.75.. 


. .. 90.00 


29. 3 !>.m. 


pi.. 91.60 


28.80.. 


. .. 92. 3o 



Solid 
Phase. 



2H; ] PO 4 .1[ : ,0 



Cms. IT 3 PO, 

per 1 00 gins. 

t". snt. sol. 

28.28 ...... 9^.72 

27.36 ...... 93.33 

9.6.08 ...... 93.74 

20. DO (Kuli'C.l. 94.75 

'25.88 ...... 95. 2S 

27 . 3o ...... 95 . 56 

28.38 ...... 95.86 

29 . 90 ...... 96.18 

3*1.96 ...... 96.80 

34.06 ...... 97-4<> 

36 . i 5 98 . oo 



Solid 
Pliasi*. 



-HH,PO v 



42.35m.pl... 100.00 

The authors failed to find the decihydrate reported by Smith and Menzies, 1909 

100 gms. sat. solution of 2H 3 P0 4 .H 2 in water contain 85.95 g ras * ^3^4 
at 25. (Grube and Staesche, 1927.) 

FREEZING-POINTS OF AQUEOUS SOLUTIONS OF PHOSPHORIC Acir>. (Ross and Jones, 1925.) 

Gms. H 3 P0 4 per Gms. ir a P0 4 per 

t*. 100 gms. sat. sol. Solid Phase. t". 100 gms. sat. sol. Solid Phase. 



PO 



- 5.. 

-10.. 



-20.. 

-25.. 



17.5 

27.0 
34.0 

38.o 
42.0 



Ice 



35 

45 

60 

75 

85 (eutec.).. , 



47-5 
5i .o 
55.o 
59.5 
62.5 



Ice 



SOLUBILITY OF ORTHO PHOSPHORIC ACID IN ETHYL ETHER. 

(Rublnowltach and J&toubaohn, 1923.) 



17.2 



30.0 
28.4 
27.5 
25.2 
23.9 
22. o( Eutec. 

25.2 

2 8.2(m.pt.) 

27.5 



Otas. H 3 P0 4 per 
100 0R8. SAC. sol. 

82.50 
83.48 

pt.) 8^.20 
84.38 
84.96 
87.00 
87.48 
87.70 



I 

88.05 
88.10 
88.80 
88.94 



Solid 


.0 * 


is. H^0 4 per 


Solid 


Phase 


C 100 


gins. sat. sol. 


Phase 


W, C e H 6 


) 8 25.5 


89.10 6H, 


5 po 4 <cyi 


II II 


22.1 


89.50 


11 M 


II II 


17-5 


89.85 


M 


II 


16.0 (Eutec. 


) 90.10 


" * H 3 P 


II 


16.9 


91-7 H 3 


.P0 4 


II 


17.7 


92.5 


*ll 


It 


21.0 


95.10 


II 


II 


23.4 


96.17 


It 


6!(PoW 


OJ 2 2 6. 5 
) 2 28.3 


97-20 
97.85 


II 
It 


*" It 


28.7 


97.93 


II 


" 


30.1 


98.50 


It 


II 


38.4 


1 00 . 00 


It 



H HYDROGEN 



594 



Freezing-point data are given by King and Walton, 1931* for each of the 
following mixtures 



H 3 P0 4 * CH COOH (acetic acid) 

" " + C ? H 5 COOH (Propionic acid) 
+ C 3 H 7 COOH (n Butyric acirt) 

11 + CH (CH ) COOH (n Caproic acid) 

" + C H COOH (Ben zoic acid) 

" + Cfl 7 OOCOOH (Pyruvic acid) 

" + CJLC1COOH (Monochlor acetic, acid) 

" + CH a,H_COOH(Phenylaacetic acid) 



C H CHO (Benzaldehyde) 
cf? 3 OC fi H 4 CHO (Anisaldehyde) 
C C H,COCH 3 ( Acetophenone) 
C^uXyyBenzo aceto 

phenone) 
C H OH (Phenol) 
CJLOH.OCIL (Guaicol) 
CH*CH:CH.DCO (Cumarin) 



PyroPHOSPHORIC ACID H 4 P 2 7 . 

SOLUBILITY IN WATER. (Giran, 1908; see note on preceding page.) 

Solid Phase. 
Ice -fl^PA.ilHjO 



t". 


Gms. ELJPA per 100 
Gms. Sat. Sol. 


-75 
+26 m. pt. 

23 

61 m. pt. 


59 
86.8 
88.8 

IOO 



4-H4PA 
EUPA 

HypoPHOSPHORIC ACID H 2 P03.H 2 0. 

100 gms. sat. solution in water contain 81.8 gms. H 2 P0 3 at the m. pt., 62, of 
the hydrated compound, HjPOs.HjO. (Rosenheim and Pritze, 1908.) 



HYDROGEN 


STTLFIDE 


H 2 S. 
SOLUBILITY IN 

(Winkler, 1906, 


WATER. 

1912.) 








r. 


Abs. Coef, /9 


q. 


t. 


Abs. Coef. 


q. t. Abs. Coef. 0. </. 





4.621 


0.699 


25 


2.257 


0-334 


60 


1. 176 


0.146 


5 


3-935 


Q-593 


3 


2.014 


0.295 


70 


1 .010 


0.109 


10 


3.362 


o-505 


35 


1.811 


0.262 


80 


o.go6 


0.076 


IS 


2.913 


0.436 


40 


1.642 - 


0.233 


90 


0-835 


0.041 


20 


2.554 


0.380 


50 


1.376 


0.186 


IOO 


0.800 






Abs. Coef ft shows the vol. of H S (reduced to o & 76omm) absorbed 
by i vol. of H 2 when the pressure of the gas without the tension of 
the liquid amounts to 76omm. 

q is the weight of H 2 S in grams which is taken up by 100 grams of 
H g O at the given temperature and total pressure (partial pressure of 
gas * vapor pressure of the liquid) is 76omm. 



595 HYDROGEN H 

THB SOLUBILITY OF HYDROGEN SULPIDB IN WATER AS MBASURBD BY THE 
VAPOR PRESSURES OF THE SOLUTIONS. 
(Wright and Maass, 1932.) 

A new type of glass diaphragm manometer was used for determination of 
the equilibrium pressures of known mixtures of Hi S * H 0, confined in 
an all glass cell. This obviated stray reactionl betwlen the gas and 
Hfj or stopcock grease. The results show that Henry's Law is not strictly 
obeyed . J 



60 



Pressure 


in pro. Hg 


/__ 


' Parti al A 


274-5 


268.0 


560.0 


553-0 


&38.0 


831.0 


1176.0 


1169.0 


303.8 


294.7 


615 


606 


914 


90S 


1279 


1270 


1567 


1558 


2112 


2103 


363.8 


345-4 


724 


707 


1067 


1050 


U83 


1466 


l8l7 


1800 


2454 


2437 


422.8 


391.3 


830 


798 


1219 


1187 


1674 


1640 


2052 


2020 


2785 


2753 


486.5 


431.6 


93 H 


879 


1370 


1315 


1853 


1798 


2278 


2223 


3095 


3040 


652.2 


503.3 


1162 


1013 


l68l 


1532 


2213 


2064 


2731 


2582 


3707 


3558 



On. Hols. H, 


? S per liter of 

5._V\_ 


Partition Coef. 


'Vapor PhaeTfyj"" 


AQ. Solutlon(s) A 


s/v 


0.0155 


0.0635 


4.09 


0.0321 


. 1 3 02 


4.06 


0.0484 


0.1910 


3.94 


0.0685 


0.2682 


3-92 


0.0168 


0.0597 


3-56 


0.0346 


0.1220 


3-52 


0.0518 


0.1801 


3-47 


0.0731 


0.2511 


3-44 


0.0900 


0.3060 


3-40 


0.1221 


0.4099 


3-36 


0.0190 


0.0528 


2.78 


0.0390 


0.1074 


2.76 


0.0581 


0.1594 


2.74 


0.0816 


0.2188 


2.68 


0.1005 


0.2696 


2.68 


0.1373 


0.3642 


2.66 


0.0208 


0.0470 


2.26 


0.0425 


0.0955 


2.25 


0.0636 


o. 1413 


2.22 


0.0882 


0.1932 


2.19 


0.1091 


0.2398 


2.20 


0. 149& 


0.3247 


2.17 


0.0222 


0.0426 


1.92 


0.0454 


0.0858 


1.89 


0.0682 


0.1260 


1.85 


0.0937 


0.1722 


1.84 


0.1162 


0.2149 


1.85 


0.1603 


0.2921 


1.82 


0.0243 


0.0359 


1.48 


0.0492 


0.0730 


1.48 


0.0747 


0.1045 


1.40 


0. 1010 


0. 1440 


1.42 


0.1269 


0.1777 


i .40 


0.1762 


0.2426 


1.38 


system H^S + 


H g O are given 


by 



The FT and the Px curves for the system H,S 
Sheffer, 1911. 

SOLUBILITY OF HYDROGEN SULFIDE IN WATER AND IN RUBBER. 
( Vcnable and Fuwa, 1922. ) 

The gas dissolved by a given amount of air free rubber was pumped out with a 
lopler pump and measured over mercury. 

100 cc. H 2 O dissolve 243 cc. (at o<> and 760 mm) H 2 S at 21" 
Rubber 273 cc. ( ) 



H HYDROGEN 59 6 

SOLUBILITY OF HYDROGEN SULFIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID 
AT 25. (Kendall and Anderson, 1921.) 



Normality 
of aq. II 01 
solutions. 

o.o(=H. 2 0). 
o.i348*." ... 
0.2828 ..... 
o 63o8" . . . 


Cc.H 2 S 
Cm. mols. iat o uud 700 mm.) 
II 4 S dissolved Normality 
per litei bv i cc. sat. sol. of aq. fl 01 
sat. sol. (at "0 mm. pressure). solutions. 

o 1028 '2. '266 2.498.. 


Cc. H a S 
Cm. mols. (nl and 7<o mm.i 
H t .S dissolved 
per liter by 1 cc. sat. sol. 
sat. sol. i at 7fiO mm. pressure). 

. . . . o. io3o 2.281 


0.1018 2.253 3.o4o.. 


. . . . o. io34 2.291 


o 1016 2.247 3.3o8.. 


. . .. o. io3g 2.3oi 


o 1016 2.25o 4-4io.. 


0.1076 2.384 


i i 80 . . 


O 10-20 2 . 260 4 874 . 


. . . . (). IOOO 2.4 1 3 


1.848 


0.1026 2.272 
HYDROGEN SULFIDE IN AQUEOUS SOLUTIONS OF HYDRIODIC 

ACID AT 25 AND 760 MM. TOTAL PRESSURE. 

(Pollitzer, 1909.) 

(ims. i>cr Liter. Mols. per Liter. Grns. per Liter. 


SOLUBILITY OF 

Mols. per Liter 


'IH'J. IHIj. [H 2 SJ. * ' HI. H 2 S. [H']. (HIJ. 
0.20 0.1040 3.54 4.71 4.38 

1,23 i. oi o.in 129.2 3.78 5.33 5-005 

1.74 I.5I O.II3 193.2 3.85 6.06 5.695 
2.l8 1.93 0.125 246.9 4-26 7.33 6.935 
2.92 2.64 0.138 337.8 4.70 9.75 9-21 
3.71 3.42 0.142 437.5 4-84 


[Hs'Sj: HI. H,S. 
0.163 560.4 5.55 
0.165 640.3 5.62 
0.181 728.6 6.17 
0.197 887.2 6.71 
0.267 1179 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 H 2 S and CH 3 OH and H 2 S and 
O are given by Baurne and Perrot, 1911, 1914. 



SOLUBILITY OF HYDROGEN SULFIDE IN AQUEOUS SALT SOLUTIONS AT 25. 

(McLauchlan, 1903.) 

NOTE. The original results are given in terms of j- which is the iodine titer (/) 

*o 

of the H2S dissolved in the salt solution, divided by the titer (/ ), of the r^S 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 H> absorbed by i vol. of aqueous solution. 



Solution. 

wNHJBr 



Grams Salt 
per Liter. 



98 

53-4 
80 

33 

16.5 
77.1 
60. i 
18.22 
24.52 
150 
450 
Pure C3H6(OH) 3 1000 



n(NHj)jCO 



n C 4 H 6 (\ 



L 
k 

i 

0.96 

0.99 

0.82 

0.91 

i .09 

i .02 

0-975 
0.905 

o.Q44 
0.858 
0.863 



Vols. H 2 S 
per i Vol. Sol. 



.61 

,40 
58 
.14 

37 
.84 
.66 

54 
.36 
.46 
.24 
.26 



**>*. ssftg 


I Vols. H L S 
TQ per i Vol. Sol. 


nKBr 


iiQ 


o.945 


2 


47 


wKCl 


74- 




o 


.853 


2 


. 22 


nKN0 3 


101 




o 


Q*3 


2 


-38 


J n K 2 S0 4 


43- 


5 





.78 


2 


.04 


i n K 2 S0 4 


21 . 


7 


o 


.89 


2 


32 


nKI 


166 




o 


.98 


2 


56 


wNaBr 


103 




o 


035 


2 


-44 


wNaCl 


58- 


5 


o 


.847 


2 


.21 


JwNaCl 


29, 


, 2 


o 


93 


2 


.42 


nNaN0 3 


85 




o 


.893 


2 


32 


J n Na 2 S0 4 


35- 


, 5 


o 


73 


I 


.90 


iwNa 2 S0 4 


17- 


S 





.853 


2 


23 



Similar data are also given for the solubility of HjS in aq. CzHgOH solutions 
and in aq. CH 3 COOH solutions at 25. 



597 



HYDROGEN H 



SOLUBILITY IN WATER AND IN ALCOHOL AT t AND 760 MM. PRESSURE. 

(Bunsen and Carius; Fauser, 1888.) 
In Water. In Alcohol. 



r. 




i Vol. HoO Absorbs. 


0. t). i Vol. Alcohol Absorbs. 





4-37 Vols. H 2 S (at o and 760 mm.) 4 


.686 


o 


.710 


17 


. 89 Vols. H 2 S (at o and 760 mm.) 


5 


3 


-97 


4.063 


o 


.615 


14 


.78 


" 


10 


3 


59 


3 


.520 


o 


530 


II 


.99 


" 


15 


3 


-23 


3 


.056 





.458 


9 


54 


u 


20 


2 


.91 


2 


.672 


0.398 


7 


42 


tt 


25 


2 


.6r 










5 


96(24) 


u 


30 


2 


-33 








. . . 








35 


2 


.08 
















40 


I 


.86 

















For definition of and q see Solubility of Hydrogen Sulfide in Water. 
SOLUBILITY or HYDROGEN SULPIDE IN SEVERAL SOLVENTS AT 20 AND 76omm. 

(Bell, 1931.) 

The solvents were saturated by bubbling H?S through them for about 3 
hours, using some 8-10 times as much gas as required for saturation. 
The dissolved gas was determined by displacing it with a current of 



CO free air and absorbing the 
containing an excess of 30$ N 2 



S in a known volume of normal NaOII 
above tnat required for oxidation to 
2 



60-70 and the excess of alkali was titrated with normal HC1. 



Hexane 6.30 
Octane 6.80 
Dodecane 5.71 
Cetane 5.05 
Cyclo Hexane 7.50 
Carbon tetrachloride 10.79 
Renzene 15.68 
Toluene 16.90 
Tetra chlor Ethylene 8.90 
Tri chlor Ethylene 13.16 


0.0341 
0.0440 
0.0513 
0.0578 
0.0338 
0.0419 
0.0563 
0.0672 
0.0372 
0.0482 



Solvent S X 

Penta chlor Ethane 10.63 0.0514 

Bromoform 16.76 0.0581 

Ethyl bromide 17.80 0.0608 

Chloroform 32.8 0.103 

Bromo Benzene 12.92 0.0376 

Chloro Benzene 13.80 0.0388 

Tetrabrom Ethane^*) 9.49 0.0446 

Tetra chlor EthanejOi6.66 0.0702 

Ethyl bromide 43.3 0.126 

Ethylene chloride 23.0 0.0719 

S = the partition coefficient of 1LS between the liquid and the vapor; 
that is S = C (the gm. equiv. per liter) r 0.0417, since S/C = 22.4 x 

293/273* 

X - the Mol. Fraction Solubility calculated en the assumption that the 

densities obey the ideal mixture law. 

At pressures between o and 15 Atmospheres, the Solubility of M 2 'S in 
Gas Oil (d = 0.8319 and vapor pressure of 2mm at 25) is expressed by 
the equation y = 4.17 (x + 1.7). 

At pressures between o and 9 Atmospheres, the Solubility of H 2 S in 
fleayy Naphtha (d = 0.8003 an '* vapor pressure of 8omm at 25) is expressed 
by the equation y 5-5(x). 

In these equations y = Volume of H 2 S at 25 and i atm. dissolved per 
1 vol. of liquid. 

X = Absolute pressure in atmospheres. (Frolich, Touch, Hogan and 
Peer, 



H HYDROGEN 59 

HYDROGEN SULFIDE 

Freezing-point Data have been determined for the following mixtures' 

H 2 S + CC1 4 (Biltz and Brautigam, 1927.) 
tf + cs, 
" + S0 2 

" + NH 3 {Sheflan and McCrosky, 1932.) 

CH 3 OH (Baume & Perrot, 1914; Baume et al, 1914.) 

e (Baume & Perrot, 1914.) 



HYDROGEN Di and TriSULFIDES H 2 S g and H 2 $ 3 . 

Freezing-point Data for mixtures of H 2 S 3 4 S are given by Butler and 
Maass, 19301 and for H S 3 * S by Walton and Whitford, 1930.) 



HYDROGEN SULFATE (Sulfuric Acid) HgSO^ 

SO 

FREEZING-POINTS OP MIXTURES op SULFURIC ACID AND WATER. 

(Hfilsmann and Blitz, 1934.) 

The many difficulties which interfere with the accuracy of determina- 
tion are described. The temperatures were measured with a thermoelement. 
The authors' original results were plotted and the following values read 
from the curves. 



..0 


Qns. H 2 S0 4 per Solid 


Ons. H^SO 
t ?. 4 


per Solid 


t 


100 0ns. sac. sol.- Phase 


100 gns. sat. 


sol. Phase 


-4.0 


30.0 Ice 


-47.2(Eutec)68.o 


H P SO A .4H 2 + HJ30 


-15-0 


20.0 " 


-45 69.0 


H 2 S0 4 .2H ? 


-35-0 


30.0 " 


-42 70.0 


M 


-55-0 


35-0 


-40 71.5 


" 


-72.i4(\ 


Eutec) 3 6.s "+H 2 SO .8Hp 


-39 (m.pt.)7 3 .i 


" 


-67.5 


37.2 H SO .8H 2 


- 39 .5(Butec)73.5 


" * H P SOAO 


-63.7 


37.8 * 


-30 74-5 


H 2 S0 4 .H ? 


-62.0 


38.2 "+H 2 SCL.6U 2 


-20 76.0 


" 


-60 


38.5 H 2 S0 4 .6H 2 


-10 78.3 


" 


-58 


39.0 


8l.O 


" 


-55 


40.5 " 


+8.5(m.pt . 184.5 


M 


-54 


42.0 "+H 2 S0 4 .4HpO 


o 88.5 


II 


-50 


43.5 H ? S0 4 .iJl 2 


-10 91.0 


M 


-40 


48.0 ' " 


-20 92.5 


II 


-30 


5S.o 


-35.5(Eutec)93.$ 


" * " 2 so 4 


-28.5< 


n.pt.)57.6s 


-20 95-5 


H S0 4 


-30.0 


60.0 " 


-10 97.0 


'n 


"35.0 


64.0 


o 98.5 


" 


-40.0 


66.0 


+10.49 100.0 


n 



599 

SOLUBILITY OF SULFURIC ACID IN WATER, DETERMINED BY THE 
FREEZING-POINT METHOD. 



HYDROGEN H 





Gms. 






Gms. 






H 2 SO< 


Gms. SO* 




H 2 S0 4 


Gms. SO 3 


t". 


per 100 


per loo Gms. Solid Phase. 


f. 


per 100 


per 100 Gms. 




Gms. 


Sat. Sol. 




Gms. 


Sat. Sol. 




Sat. Sol. 






Sat. Sol. 




10 

20 


16.25 
24 


I3-25(I)(S) Icc 
I9.5d)(2)(3) " 


10 

o 


77.75 
80.25 


63.5 (3) 
65.5 (2) 


30 


28.5 


23.25 (2) 


+ 8.35* 84.5 


68.98 (2) 


"40 


3L25 


25.5 (2) 


8.81 


84.5 


68.98 (l) 




33-5 


27.25 (l) (2) < 





88.25 


72 (2) 


60 


35.25 


28.75 (l) 


20 


91-5 


74-75 (i) 


.70 


36.75 


30 (2) 


30 


92.5 


75.5 d) 


75 


38 


31 (2) ' +S0 3 . 5 H 2 


-38 


93 


76 (2) 


70 


39 


31.75 (2) S0 3 .sH 5 O 




93-75 


76.5 (4) 


60 


4L5 


33-75 (2) " 


20 


95- 2 5 


77-75 (4) 


50 


44 


36 (2) 


10 


96-25 


78-5 (0(4) 


-40 
-30 


47-75 
53.25 


39 (2) " 
43-25 (2) " 




-j-io 


97-75 
99-75 


79-75 (4) 
81 (4) 


-25* 


57.65 


47.06 (2) " 


10,35 


100 


81.62 <x)(3)<7 


.30 


61 


49.75(2) " 


10 




82 (4) 


-40 


65-25 


53.25 (2) " 







83.25 (4) 


-60 
70 


70-75 
73.25 


57-75 (3) " (unstable) 
59.75(3) " " +S0 3 . 2 H 2 


10 
12 




84.5 (4) 
85 (4) 


-60 


73.50 


60 (3) S0 3 .2H 2 ^unstable) 


10 




85.25 (4) 


-50 


74.25 


60.5 (3) 


O 




86 (4) 


-50 


68 


55-5 (2) S0 3 . 5 H 2 0+S0 3 . 3 H 2 .-fio 


86.75(4) 


45 


68.5 


56 (6) S0 3 . 3 H 2 


20 


. . . 


87-5 (4) 


-40 


71 


58 (6) 


30 




88.5 (4) 




* 73-14 


59.69 (6) " 


36* 




89-89 (4) 


-40 


74.25 


60.5 (6) 


30 




90-5 (4) 


-41 


74.75 


6 1 (6) " -fS0 3 .2H 2 O 


20 


. . . 


9i-5 (4) 


-40 


74.75 


6 1 (4) SO,.2H 2 


IO 




92.25 (4) 


-30 


75.25 


61.5 U) 


6-5 




93 (4) 


-20 


76.5 


62.5 (3) 









Solid Phase. 



SO,.2H 2 



SO 3 .H 3 O 



SOj-iHaO 



SO 



* m. pt. 

(i) =Pfaundler and Schnegg (1875); (2) = Pickering (1890); (3) =Thilo (1892); Pictet (1894); (4) 
= Knietsch (1901); (5) = Riidorff (1862); (6) Biron (1899); (7) = Marignac (1853). See also Pickering 
(1890-91); Lespieau (1894) and Giran (1913). 



SOLUBILITY OF SULFURIC ACID IN BENZENE SOLUTIONS OF VALERIC 
ACID AT 1 8. 

(Gurwitsch, 1914.) 

The mixtures were shaken with excess of 95.8% HiS04 at o and then brought 
to equilibrium at 18. 



Gms. Valeric 

Acid per 100 

Gms. Valeric 

Acid+Benzcne. 

o=Pure benzene 

0.584 

i .62 

3-64 
7 .60 

17-5 



Gms. H 2 S0 4 
per 100 Gms. 

of the 
Sat. Solution. 

O 
0.052 

o. 104 
0.226 

0.378 
0.454 



II HYDROGEN 600 

EQUILIBRIUM IN THE SYSTEM SULPURIC ACID, NITROBENZENE AND WATER AT 17. 
(Bailey and Hilton, 1936.) 

Weighed quantities of two of the components were nixed and the third 
(usually water) added until opalescence appeared. A perfectly sharp end 
point was usually obtained. 

On. Mols. per 100 gj. Mola. On. t Mols. per 100 SB. Mols. Om. Mols. per 100 gm. Mols. 

of the three Constituents of the three constituents of the tnree constituents 

0.054 84.9 15.0 6.52 44.6 48.9 46.3 17.1 36.6 

0.084 80 7 19.2 8.9 42.1 49.0 48.4 16.7 34.9 

0.32 66.2 33.5 15.1 36.0 48,9 64.1 10.2 25.7 

0.88 57.4 41.7 17.1 345 48.4 76.6 5.5 17.9 

1.59 53*7 44-7 19.2 32-5 4-8.3 86.4 3.0 10.6 

2.34 51.3 46.4 26.3 27-5 46.2 97.6 0.41 2.02 

4.24 48.0 47.8 32.7 23.5 43.8 "98.6 1.4 

* 0.03 99-99 

* These two results by Davis, 1916 

Experimental determinations by the method of Alexieff of Equilibrium 
in the System Sulfuric Acid, Phenol and Water are given by Svecova, 1938- 

Results for the distribution of H g S0 4 between Water and Phenol, at 
17 are given by Wosnessersky and Astachow, 1925. 

Freezing-point data have been determined for the following mixtures: 

f! 2 S0 4 + ZnS0 4 and other sulfates (Kendall and Davidson, 1921.) 

" + Phenol (Kendall and Carpenter, 1914; Kendall and 

Landon, 1920; Kendall and Davidson, 1921.) 
" + Nitrobenzene (Masson, 1931.) 
" + Amyl alcohol (Archibald, 1932.) 
" + Tertiary Amyl Alcohol " " 
" + n Butyl Alcohol " " 
- " * Acetic acid and long (Kendall and Carpenter, 1914; Atsuki and 

series of Organic Compounds Tsshi, 1931.) 

HYDROGEN SELENEDE H 2 Se 

SOLUBILITY IN WATER. 

(de Forcrand and Fonzes-Diacon, 1902.) 

t. 4 9.65 13-2 22.5 

Vol. H 2 Se (at o and 760 mm.) dissolved \ 7 .- 7 1T . 
SeO penvol.H 2 j 3 " 77 3 ' 4S 3 ' 3 ~' 7 

SOLUBILITY OF HYDROGEN SELENIDE IN WATER AND IN AQUEOUS SOLUTIONS 
OF HYDRIODIC ACID AT A PARTIAL PRESSURE OF H 2 Sc OF 760 MM. 
( Me Amis and Felsin#, 1!)25. ) 

Solubility in Water. Solubility in Aq. HI Solut. at 25. 

Cc. II,, Sc Cc. IIj Se 

Mols. H* So (alO'andTfiOmm.) Mols. HI Mols. H*Se ( at and 7dO mm. 

t. per liter sal. sol. per liter sat. sol. per liler. per lit or sat. sol. per lller sat. sol. 

14.6.. . o. 09789 v>.i94 o.ao 0.08478 1900 

1 5.0 0.0()6li 2 1 54 0.40 0.08634 IQ3/) 

25.o o.o84i5 1886 2.78 o.iioiy. 2468 

25 . 6 .... o . 08277 1 855 
35.o 0.07317 1640 



60T 



HYDROGEN H 



HYDROGEN SELENITE (Selenious Acid) H.SeO,. 

<c 3 

SOLUBILITY IN WATER. 

(Etard, 1894.) 



1. 
IO 

o 

+ 10 

20 



Gms. H 2 ScO 3 per 
100 Gms. Solution. 

42 .2 

47-4 

55 

62.5 



25 
30 
40 

50 



Cms. HoScO.i per 
100 Gms. Solution. 

6 7 - 
70.2 

77-5 
79.2 



60 
70 

So 
90 



Gms. H 2 Se0 3 per 
too Gms. Solution. 

79-3 
79-3 
79-3 
79-4 



HYDROGEN SELENATE (Selenic Acid) H g Se0 4 . 

SOLUBILITY IN WATER, DETERMINED BY FREEZING-POINT METHOD. 

(Kremunn and Hofmeier, 1908.) 





Gms. H,Se0 4 




t. 


per 100 Gms. 


Solid Phase. 




Sat. Sol. 







O 


Tee 


10 


21 


" 


20 


30 


" 


-30 


36 


" 


-40 


40 


" 


- 5 


42-5 


" 


-60 


45 


" 


-80 


48 


" 


95 Eutec. 


SO 


" +H,Se0 4 .4l 


-80 


52 


H,Se0 4 . 4 H 2 C 


-70 


54 


" 


-60 




" 


51 m. pt. 


67 






~55 

-65 Eutec. 
-50 
20 
o 

+ 20 

26 m. pt. 

20 

16 Eutec. 

30 
40 
So 
60 

FREEZING-POINTS OF MIXTURES OF SELENIC ACID AND SULFUR TRIOXIDK. 
( Meyer and Statcc/ny, 1922.) 

A diagram is given and the following numerical data for the principal points 
of the diagram. 



Gms. HjSeO 4 




per 100 Gms. 


Solid Phase. 


Sat. Sol. 




71-5 


H a Se0 4 . 4 H,0 


:. 74 


" -r-H'>SeOj.I 


75-5 


HoSA-H/O 


79 


** 


81 


" 


85 


" 


88 





Qi 


;; 


93 


H 2 SeO< 


94-5 


" 


96.5 


" 


100 


** 



SeO 



t". 
58.... 

-I'Jt Huh 
- 6.6 no 



(Jms. SO, per 
1 00 gms. mixture. 



o.o 
23. o 
35. o 



Solid Phase. 

ILSeG 4 



II 2 SeS0 7 

HYDROGEN SILICIDE H Si 

One liter of Cyclo Hexanol(C ( 
76snim. (Cauquil, 1927.) 



-i ILSeSOy I 9 . PL 
-7.0 Kutcc. 



(ims. S0 3 per 
1 00 #ms. mixture. 

40.4 

53.o 
63.9 



Soliil IMi/isc. 
II a S<'S0 7 "Hir.,SeS..O U) 

U 2 SeS,0 10 

-i- SO., 



9700. HSi at 26 and 



Si 



HELIUM He. 

SOLUBILITY OF UKLIUM IN WATKU. ivon Ani.ropolT, r.>-J5.) 

New dcl.crminations made with a highly relincd apparatus and with the greatest 
possible accuracy, gave the following values, which an* expressed in terms of the 
Bunscn absorption coefficient, as modified by Kucncii to show the volume of gas 
(reduced to o and the 760 mm) dissolved by i.o gm. of H 2 0.. 

t" ii". 10. iiii'; :;i". .H)". JiO". 

Absorption coef 0.0097 ' ()( >i)9 o.oioo o.moi o.oio3 0.0108 



HELIUM 602 

SOLUBILITY OF HELIUM IN WATER. (Cady, Elscy and Berber, 1022.) 
The following very carefully determined results are given in terms of the Ostwaldf 

Q.'lS I X V 

solubility expression a = ' s 1 ? in which V = the volume of H 2 0, V 1 = the 

volume of helium absorbed by V volumes of H 2 and T = temp, on the absolute 

scale. 

t '-i'.o. 10. 23. no. 

a 0.00937 0.00896 0.00860 0.00817 

According to Venable and Fuwa, 1920, 100 cc. of H^ dissolve 1.4 cc. He (reduced 
to o and 760 mm.) at 21. These authors also found that 100 cc. of rubber 
dissolve about i.o cc. of helium at 21, as determined by pumping out the gas 
with a Toplcr pump and measuring it over mercury. 

SOLUBILITY op HELIUM IN VATER. 

(Lannung, 1930.) 

The results are in terms of the Bunsen Absorp. Coef . j3 and the Ostwald 
Solubility Expression ] . 8 - iff * w l Po* where W and w are the volumes 

WL x P 

of He originally introduced and remaining after absorption (reduced to 
o and 76omm). WL is the volume of H 2 at the temp, of saturation. P is 
the partial pressure of He in mm Hg and P is 760 mm. ] - the equilibrium 
distribution ratio of the volume concentration of He in the solution and 
in the vapor phase. 

ft I 

15 0.0089 0.0094 

20 0.0088 0.0095 

2$ O.OOS? 0.0095 

30 0.0086 0.0095 

37 0.0084 0.0095 

The older results of Rstreicher, 1899, are considered to be too high 
due to inaccuracies in the method of determination. 

SOLUBILITY op HELIUM IN WATER AT PRESSURES UP TO 1000 ATMOSPHERES. 

(Wlebe and Oeddy, 1935.) 

The authors used a simple bubbling-type of apparatus made of a steel 
cylinder with pressure valves. Equilibrium was approached from both 
lower and higher pressures. The helium was 99.95% pure. It was found 
that 1% N impurity had a very decided effect upon raising the solubility, 
but 0.05% was negligible. 

Partial Pressure 
of He in AtAoapherea 

25 

50 
100 
200 
400 
600 
800 
1000 

The averages of the 25 and 50 atm. values were used to compute the 
Bunsen and Ostwald coefficients. The values thus obtained were found 
to be in good agreement with the results of Cady, Elsey and Berger, 
1922* and Lannung, 1930.) 



cc H 2 ( reduced 


to o and 7flOwn) 


jjllaaolved per i.o 


gm. H?0 at: 


00 


250 


500 


750 > 


0.2322 


0.2156 


. 0.2225 


0.2442 


0.4674 


0.4332 


0.4445 


0.4892 


o . 9240 


0.8491 


0.8827 


0.9699 


1.807 


1.688 


1.734 


1.907 


3.436 


3.241 


3.358 


3.666 


4.916 


4.681 


4.844 


5.277 


6.228 


6.015 


6.248 


6.787 


7.421 


7.263 


7.536 


8.251 



603 HELIUM He 

SOLUBILITY OP HELIUM IN WATER AND IN- WHOLE BLOOD AT 38. 

(Hawkins and Shilling, 1936.) - 

The blood of oxen or dogs was oxalated with 0.02 percent oxalate and 
used immediately or chilled to nearly o and used the next day. The 
time allowance for saturation was 30 minutes. TheO capacity of the blood 
samples varied from 18 to 21.5 vol. percent. The H g O content from 0.77 
to 0.89 gro. per cc. 

Results for H g O Results for Ox and Dog Blood 

He pressure He content, He Pressure He Content 

In ran. Hg In Vol. Percent in mm. Hg In Vol. Percent 

723 0.8o 699 0.83 

1495 1.68 1466 1.70 

3025 3.41 3028 3-5^ 

4620 5.20 4556 5-59 

The solubility coefficient for He in Water is 0.085 anfl tnat f r dog 
blood was found to vary from 0.083 to 0.089 and that for ox blood to 
vary from 0.080 to 0.091. The amount of helium dissolved by whole 
blood under helium pressures varying from i to 6 atmospheres (absolute) 
was found to be directly proportional to the helium pressure in accordance 
with Henry's law. 

SOLUBILITY OF HELIUM IN AQUEOUS SOLUTIONS OF SALTS AT 25. 

(EKerlof, 1935.) 

Aqueous Qm. mols. Salt cc He (at and 760mm. > In an arot. 

Solutions of: per 1000 gm. H g o of solution containing l.o gm H.,0 

Potassium Chloride 4.72 0.0048 

Sodium Chloride 5.81 0.0043 

Lithium Chloride 6.18 0.0136 

Lithium Iodide 2.40 0.0109 

Sodium Nitrate 6.95 0.0039 

Perchloric Acid 6.89 0.0187 

Water alone o.o 0.0086 

SOLUBILITY OF A MIXTURE OF 30 PERCENT HELIUM AND 70 PERCENT 

NEON IN WATER. 

(ValenUner, 1927.) 
t 1 (Ostwald Solubility Expression) 

0.021 

17 0.015 

45 0.010 

The author has collected and recalculated all previous determinations 
of the solubility of the rare gases in water. 

SOLUBILITY OF HELIUM IN LIQUID AMMONIA. 

(Ipatjew and Teodorowltsch, 1932.) 

He Pressure cc He g (at and 760wm) He Pressure cc He g (at 0. and 760nun) 

1 in Atm. dissolved In I.QCC NH_ * In Atm. dissolved In l.occ NH, 

3 A 

-16 35-5 0.554 +20 23.3 0.465 

-10 34.55 0.521 " 38.7 0.719 

+20 5.35 0.126 25 37-7 0.750 



HELIUM 



604 



SOLUBILITY OP HELIUM IN SBVBRAL ORGANIC SOLVBNTS. 

(Lannung, 1930.) 

The results are expressed in terms of the Bunsen Absorp. Coef. and 
the Ostwald Solubility Expression (See results for the Solubility of 
Helium in Water by Lannung, 1930.) 

Results for the Solubility in: 
Methyl Alcohol 



15 
18 

20 
25 
30 
37 



0.0298 0.0314 
0.0307 0.0327 
0.0313 0.0336 
0.0328 0.0358 

0.0343 0.0381 
0.0364 0.0413 


0.0268 0.0283 
0.0275 0.0293 
0.028l 0.0302 
0.0294 0.0321 
0.0306 0.0340 
0.0325 0.0369 



0.0284 0.0300 

0.0299 0.0319 

0.0309 0.0332 

0.0331 0.0361 



Cyclohj^icanol 
- 



15 
18 
20 

25 
30 
37 



0.0165 0.0174 
0.0174 0.0l86 
O.OlSo O.O193 
0.0192 0.0210 
0.0202 0.0221J. 
0.0221 0.0251 


0.0220 0.0232 
0.0227 0.0242 
0.0236 0.0253 
0.0252 0.0275 
0.0268 0.0297 
0.0293 0.0333 



0.0100 0.0109 
0.0107 0.0119 
0.0119 0.0135 



HAFNIUM Oxy BROMIDE HfOBr g 

SOLUBILITY IN AQUEOUS SOLUTIONS OP HYDRO BROMIC ACID AT 25. 

(v. Hevesy and Wagner, 1930.) 



d ^ of 
sat. sol. 

2.0838 
1.6989 
1.4348 



Normality 



HfO 



? 






of 



of Aq. HBr per liter sat. sol. sat. sol. 



Normality Qtes. HfO g 

of Aq. HBr per liter sat. sol. 



0.354 
3.620 
6.568 



694.5 
314.5 
48.90 



1.4984 
1.7157 



8.77 
13.36 



10.60 
0.80 



HAFNIUM Acid Oxy FLUORIDE HfOF 2 .H 2 F g .2H 2 0. 



SOLUBILITY IN AQUBOUS SOLUTIONS OP HYDROFLUORIC ACID AT 25. 

(v. Hevesy and Wagner, 1930.) 



d ^ ot 
sat. sol. 

1.577 
1.537 
1.650 
1.655 
2.036 
2.040 



0.0 
0.0 
1 .06 



ity 
HBr 


Qtes. Hf0 2 
per liter sat. aol. 


d ^ of 
sat. aol. 


Normality 
of Aq. HBr 


6 


413.6 
475-6 
568.3 


2.050 
1.899 
1.902 


10.05 
15.05 
15.03 


6 
3 
3 


571.2 
892.1 
897.1 


1.394 
1.404 


20.O9 
20.O9 



per liter sat. sol. 

903.9 
733-6 
741.8 
250.6 
258.9 



Cm. mols. IirOCl 2 


JN'ormalilj 


</ of 


C,iu. mols. HfOCl a 


IXT liter sat. sol. 


a<[. II Cl. 


sal. sol. 


per liter sat. sol. 


0.167 


10.56 


1.180 


0.0801 


0. K)3 


11.28 


- 


o . i 009 


o.o53 


II.4O 





o . 06 i 9 


0.0668 









6os H AFN I UM Hf 

HAFNIUM Oxy CHLORIDE HfOCU. 

SOLUBILITY OF HAFNIUM OXYCHLORIDE IN AQUEOUS SOLUTIONS OF 

HYDROCHLORIC ACID AT 20. (von Hevesv, 1925.) 
The hafnium contained 5 per cent Zr O a . 

Normality d of 

aq. JlCl. sat. sol. 

5.04 

0.48 1.127 

9.02 1*1.54 

10.33 

HAFNIUM Ammonium FLUORIDES, Hf (NH*) a F 6 and Hf (NH 4 ) 3 F 7 . 

SOLUBILITY IN WATER. AND AQ. NH 4 F SOLUTIONR. 
(von Hevesy, 1925; von Hevesy, Christiansen and Berglund, 1925.) 

Mols. per litter 
Compound. Solvent. t. NHj. """"'" j[f 

Hf(NH 4 ) 2 F 6 Water o 1.807 0.890 

20 -jt.832 1.4^5 

Hf(NH 4 ) s F 7 o i.-iSo o.4a5 

'to 1.706 o.538 

0.922 n NH 4 F uo - 0.261 

I -97 I ^o - 0.108 

5.oi 20 0.0258 

Water 20 3 . o38 i . /I3q 



HAFNIUM Potassium FLUORIDE HfK 2 F 6 . 

One liter of aq, o. rv.5 n HF solution dissolves o. 1008 mols. Hf K. 2 F f) at 20 
5,89 o.u)4'2 

(von Hovesy, 1925; von Hevesy, Ghristia 'son and Berglund, 1925.) 

HAFNIUM PHOSPHATE Hfo"(H 2 PO. v ). 

SOLUBILITY OF HAFNIUM PHOSPHATE IN AQUEOUS SOLUTIONS OF 
HYDROCHLORIC AciD AT 50. (von Hevesy ami Kimura; 1925.) 

About o.i gm. of the compound was shaken 3 days in a thermostat and then 
allowed to stand many days. 100 cc. of the solution filtered through glass wool 
was evaporated and residue ignited and the weighed. 

Normality Wl. of Ignited ivsl<lm % (im. mols. 

of aq. HOI. from loocc. sm. sol. eumpil. p<u' liter. 

5.(j4 O.O()3l O.OOOOJ) 

lo.'.u o.oo43 o.ooorjt' 

10.48 o.oo/j(5 u.oooi3 

HYDRARGYRUM (Mercury) Hg . 

THB SOLUBILITY OF METALLIC MERCURY IK VATKR. 

(Stock, 1934.) 

By operating with the greatest possible care to remove air from the 
water and the Hg, the solubility was found to be 

0.02 to o.oay Hg per cc H 2 at 30 (y - o.ooi mg.) 

When the separation of the water from the Hg was made in the air the 
solubility rose to o.o6y or more per cc H g O. This increase is due to 
oxidation. At 85 the solubility was found to be o.jj and at 100 
o.6y Hg per cc H g O. 

Experiments were also made at 30 of the solubility of Hg in H in 
contact with air, both with and without stirring and in presence 2 of 
of oxygen. In the latter case the solubility rose to 39. 6y flg per cc 
H g O v in 2 months. Using pure red HgO a solubility of 42.^ HgO per cc 
H g O was found. Alkali hydroxide in presence of air increased the Solu- 
bility of Hg to s^y in 5% KOH and to i 3 sy iu 10% KOH, Many other experi- 
ments of a similar character are described. 



g HYDRARGYRUM 606 

HYDRARGYRUM BROMIDE (Mercurous Bromide) Hg g Br 2 

One liter sat. sol. of Hg Br in water contains 0.000039 gm. Hg 9 Br 
at 25. (Sherrill, 1903.) 

From the measured E.M.F. of the chain Hg I Hg Br 2 .KBr, C I KNO against 
I C, KCl.HggCl I Hg; E = 0.1318 - o.oooiSSt, the calculated Solubility 
Product of HgsBra is o.s^S.icT 23 at io8., i.oo.io" 23 at iq.,9 , 3.88.io~ 23 
at 19.2 5-S.io" 23 at 25 and 6.95.io~ 23 at 26.5. 

HYDRARGYRUM BROMIDE ^fercuric Bromide) HgBr 2 

SOLUBTLITY OP MERCURIC BROMIDB IN WATBR. 
(Tburneux and Pernot, 1925J above 100 Benratti, Ojedebo, Schlffers and Wunderllch, 1937.) 



t o 


Gtas. HgBr 2 


o 


ana. HgB 


ir 2 o 


Gtas. HgBr g 




per 100 gns. sat. sol. 




per 100 0ns. s 


at. sol. c 


per 100 0ns. sat. 





0.3 (?) 


50 


1.25 


173 


33-5 


10 


0.4 (?) 


60 


1.65 


185 


59.1 


20 


0-55 


80 


2.7 


187 


74-7 


25 


0-6l 


100 


4.7 


189 


88.1 


30 


0.65 


142 


12.0 


193 


92.8 


40 


0.9 


164 


22.4 


201 


96.2 



EQUILIBRIUM IN THE SYSTEM MERCURIC BROMIDE, AMMONIA, WATER AT 8-io. 

(Gaudechon, iyio.) 

The mixtures were shaken in tcrmitt entity for 21-48 hrs. Both the clear sat. 
solution and the separated and dried solid phases were analyzed. 



Initial Mixture. Sat. Solution. 
Cms. Mols. per Liter. Cms. Atoms, per Liter. 

,,,*,., A CnlSrl T>1. .__ 


HgBr,. NH,. 
0.0125 0.0250 
0.0166 0.0332 
0.025 0.050 
0.050 o.ioo 
0.0125 0.025 
0.025 0.050 
0.0328 0.0656 
0.0365 0.073 
0.050 o.ioo 

O.IOO O.2OO 

0.0180 0.036 
0.050 o.ioo 
0.050 o.ioo 

O.IOO 0.200 

0.125 0.250 
SOLUBILITY OF 

(The mixtures 
In Aq. BaBr 2 . 

Mols. per Liter. 


NH 4 Br. Hg. Br. N. 
o trace 0.0154 0.0185 (NHg 2 Br) 4 HgBr 2 
o 0.00032 0.0172 0.0202 36% " +64% NHg 2 BrNH 4 Br 
o 0.00078 0.0241 0.0251 NHgsBr.NHiBr 
o 0.0019 0-0525 0.0514 " 
0*0375 0.00178 0.0497 0.0497 " 
0.075 0.0041 0.103 0.108 " 
0.0984 0.006 1 0.133 - I 33 93% " +6% NHgBr.3NH 4 Br 
0.1095 0.0060 0.132 0:133 36% " +64% NHgBr.aNELJBr 
0.150 0.007 0.170 0.169 NHgjBr^NF^Br 
0.300 0.0124 0.333 0-33 8 
0.01875 O.oo I 0.0315 0.0318 NHg 2 Br.NH 4 Br 
0.006 0.0057 0.1172 0.1178 " 
0.150 0.0071 0.169 0.168 NHgjBr.aNH^Br 
0.160 0.0083 0.184 0.187 " 
0.306 0.0160 0.393 - " ' 
MERCURIC BROMIDE IN AQUEOUS SALT SOLUTIONS AT 25. 

(Herz and Paul, 1913.) 

were constantly agitated for eight days.) 
In Aq. CaBr* In Aq. KBr. In Aq. NaBr. In Aq. SrBr 2 . 

Mols. per Liter. Mols. per Liter. Mols. per Liter. Mols. per Liter. 


BaBr 2 . HgBr s : 

o 0.017 

0.274 0.370 
0.396 0.540 
0-579 0.759 
1.096 1.478 


CaBr 2 . HgBr 2 . KBr. HgBr 2 . NaBr. HgBr,." SrBr 2 . HgBr 2 r 
0.072 0.117 o 0.017 0.118 0.078 0.062 0.104 
0.645 0.676 0.209 0.098 0.596 0.285 0.328 0.471 
1.892 1.358 0.770 0.472 1.142 0.540 0.668 0.902 
2.479 2:766 2.380 1.360 2.448 1.276 1.401 1.770 
3-754 3-666 3.470 1.930 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. HgBr2 per liter 0.017 0.055 0.088 0.0359 0.6 n 1.407 2.096 2.339 

Data for equilibrium in the system HgBr 2 + KOH + HaO at 25 are given by 
Herz (1910). 



Soy HYDRARGYRUM Hg 

SOLUBILITY OP MERCURIC BROMIDE IN AQUEOUS SOLUTIONS OP POTASSIUM 
BROMIDE AND VICE VERSA. 
(Pernot, 1932.) 

The original results are presented only in the form of a diagram from 
which the following approximate figures were read. 



Results at o 



Results at 34 



Ons. per 100 
gms. sac. sol. 


KBr 


Hg Bg * 


0.0 


0.3 


7.5 


15-0 


12.0 


2^.0 


20.0 


31-5 


2$.0 


37.5 


30.0 


43.2 


32.5 


48.2 


32.2 


40.0 


31.8 


30.0 


32.5 


20.0 


34-0 


0.0 



Phase 




Solid 
Phase 



Results at 80 

Gkns. per 100 

gms. sat. sol. Solid 

A Hg Br \ Phase 



o.o 



0.68 



0.0 



2.7 



5.0 15.0 
+ 1.1.110.0 23,0 



KBr 



KBr 



15.0 


38.0 


19.0 


5i>o 


23.0 


48.5 


28.0 


48.0 


33.5 


55.0 


34-0 


45.0 


35-0 


30.0 


40.0 


15.0 


42.1 


0.0 



10.0 30.0 
15.0 50.0 



1.1.1 



4 KBr 



KBr 



18.5 


75-0 " + 1.1.1 


21.5 


70.0 1.1.1 


25.0 


65.0 " 


28.0 


63.0 


32.0 


62.0 " 4 KBr 


35.0 


50. KBr 


40.0 


26. " 


44.0 


15. 


48.7 


o.o " 



1.1.1 = HgBr 2 .KBr.H 2 
HYDRARGYRUM BROMIDE (ic) 

SOLUBILITY OF MERCURIC BROMIDE IN AQUEOUS 
ALCOHOL, ETHYL ALCOHOL AND OF ETHYL 

(Her/anrI Anders, jyo;.) 



SOLUTIONS OF METYHL 
ACETATE AT 25. 



In Aq. 


Methyl Alcohol. 


In Aq. 


Ethyl Alcohol. 


In 


Aq. 


Ethyl Acetate. 


CHJOH 


d 


AS Of 


Gms. 
HgBr 2 per 


Wt. % 
C 2 H 5 OH 


d 


of 


Gms. 
HgBr 2 per ( 


Wt. 


% 


, </ v of 


Gms. 
HgBr 2 per 


m 


Si 


it. Sol. 


100 CC. 


in 


Sa 


t. Sot. 


IOO CC. 


ii 


i 


Sat. Sol. 


IOO CC. 


Solvent. 






Sat. Sol. 


Solvent. 






Sat. Sol. 


Solvent. 




Sat. Sol. 


IO.6 





9857 


0.72 


. 


I. 


0022 


0.6o 







1.0022 


0.6o 


30-77 





.9588 


1.29 


20. l8 


0. 


9717 


0.67 


4- 


39 


I .0018 


0-574 


47.06 


o 


.9401 


2.52 


40.69 


0. 


9435 


1.59 


96. 


76 


I.H59 


26.69 


64 


o 


.9386 


6.85 


70.01 


0. 


9214 


6.58 


IOO 




1.0113 


14.13 


78.05 





9744 


14.66 


IOO 


0. 


9873 


22. 8l 










IOO 


I 


.2275 


50-25 



















IOO gms. sat. sol. in 95% CjH&OH (d is = 0.8126) contain 13.2 gms. HgBr* at 
, 16.53 gms. at 25 and 22.63 gms. at 50. (Reinders, 1900.) 



o, 16.53 gms. 

SOLUBILITY OF MERCURIC BROMIDE IN ALCOHOLS. 

(Timofeiew, 1894.) 

In Methyl Alcohol. In Ethyl Alcohol. In Propyl Alcohol. In Isobutyl Alcohol. 



t" 


Gms. HgBr 2 
per 100 Gms. 


t. 


Gms. HgBr 2 
per TOO Gms. 


f. 


Gms. HgBr, 
per loo Cms. 


t'. 


Gms. HgBr, 
per loo Gms. 




CH 3 OH. 




C 2 H 8 OH. 




C 3 H 7 OH. 




C,H 9 OH. 





41 .15 


O 


25.2 





14.6 


o 


4-6l 


IO 


49-5 


IO 


26.3 


10 


15.6 


IO 


5-63 


19 


66.3 


19 


29.7 


19 


15-5 


2 3 


6.65 


22 


60.9 


39 


31-9 


39 


20.8 


39 


9-58 


39 


71-3 


65 


44-5 


65 


31-3 


65 


15.80 


65 


90.8 


89 


66.9 


86.5 


42.7 






97 


I39.I 















Br 



[g HYDRARGYRUM 608 

MERCURY BROMIDE (ic) HgBr 2 . 

SOLUBILITY OF MERCURIC BROMIDE IN WATER AND IN AQUEOUS SOLUTIONS 
OF GLYCEROL AT 25. ( Moles and Marquina, 1924. ) 

Oms. HBr s per 
Solvent. r/as of sal. sol. 100 gins, solvent. 

Water i.oo*3 o.6i35 

Aq. 25.0 / glyceroi i.o65i 0.9840 

75.2 1.2204 3.456 

99-2 i.4ooo 16.687 

SOLUBILITY OP MERCURIC BROMIDE IN METHYL ALCOHOL AND IN ETHYL ALCOHOL. 

(Lloyd, Brown, Olynwyn, Bonnel and Jones, 1928.) 
Results for Methyl Alcohol Results for Ethyl Alcohol 

Ons. HgBr ? per Solid 

100 gms. C^HjcOH Phase 



f. 


Qua. HgBr g per Solid 




t 


100 gms. CHgOH Phase 


t 


10 


53.5. HgBr 2 .CH 3 OH 


. 


20 


65-3 


10 


22 


70.3 


20 


2? 


71.6 HgBr 2 


30 


30 


72.1 " 


40 


40 


76 . o " 


50 


50 


81.9 


60 


60 


85.1 


70 



27.3 HgBr,, 

28.2 
28.6 

31.6 

34.0 " 

36.2 " 

42.3 " 
46.3 " 

SOLUBILITY OP MERCURIC BROMIDE IN METHYL ALCOHOL AND IN ETHYL ALCOHOL. 

(Malhotra, 1929.) 

Except in a. few cases the determinations were made by the synthetic 
method. 

Results for Methyl Alcohol Results for Ethyl Alcohol 

of d^ = 0.7961 = 99.88 Wt.% CII 3 OH of 87.73 Vt.% C ft H B OH 

Q Oms. HgBr g per Oms. HgBr g per 

1 100 gms. CH 3 OH C 100 0ns. solvenc 

22.1 67.62 32.9 17.22 

27.4 68.8l 42.13 21.44 

30.8 70.25 45.20 22.91 

36.1 73-31 49-07 25.35 

49.8 84.43 55.85 28.61 

6l.6o 31.84 

68.97 37.il 

Results for Ethyl Alcohol 
of dl = 0.7943 = 99.78 Wt.% C 2 H g OH 

Oms. HgBr 2 per Q tea. HgBr 2 per 

C 100 gS. Cj^^H ' C 100 9. CgHgOH 

34-55 
35.87 
37.80 
39.80 
40.63 
43-10 
60.15 



0.0 


24.04 


44.80 


16.15 


26.25 


48.60 


24.95 


28.40 


53-20 


29.15 


29.28 


58.00 


31.35 


30.05 


60.15 


34.30 


31.29 


64.80 


41.60 


33.53 


79.25 



HYDRARGYRUM BROMIDE (ic) 



6og 



HYDRARGYRUM Hg 



SOLUBILITY OF MERCURIC BROMIDE IN MIXTURES OF ALCOHOLS AT 25. 

(Herz and'Kuhn, 1908.) 

In Mixtures of Methyl In Mixtures of Methyl In Mixtures of Ethyl and 
and Ethyl Alcohol?. and Propyl Alcohols. Propyl Alcohols. 



% CH 3 OH 


Cms. 
d * ol HgBr 2 per 


%C 3 H 7 OH rf of 
in *" 


Gms. 
HgBr, per 


% C S H 7 OH <r of 
in * 


Gms. 
HgBrs per 


Mixture. 


Sat. Sol. 


100 cc. 
Sat. Sol. 


Mixture. 


Sat. Sol. 


100 CC. 

Sat. Sol. 


Mixture. 


Sat. Sol. 


IOO CC. 

Sat. Sol. 





o 


-9873 


22.8 


o 




1.227 


50.20 








-9873 


22.8o 


4-37 


o 


.9032 


23.1 


ii . 


.11 


I I9S4 


47-28 


8.1 


'O, 


.9802 


22.25 


10.4 


I 


.009 


25-4 


23 


.8 


I.IS24 


41-53 


17-85 


o. 


,9740 


21.06 


41.02 


I 


.080 


33-3 


65 


.2 


1.0257 


25.30 


56.6 


o. 


.9487 


17.63 


80.69 


I 


185 


45-7 


91 


.8 


0.9437 


16-35 


88.6 


o 


.9269 


14.76 


84.77 


I 


193 


46.8 


93 


75 


0.9368 


15.86 


91.2 


o 


9239 


14.64 


91.25 


I 


,211 


48.6 


96. 


.6 


0.9275 


14.66 


95-2 





.9227 


14.06 


TOO 


I 


.227 


50.2 


100 




0.9213 


13.78 


IOO 


o 


.9213 


13,78 



SOLUBILITY OP MIXTURES OP MERCURIC BROMIDE AND MERCURIC 
CHLORIDE IN ALCOHOL AT 25. 

(Van Pelt, Jr.. and de Boer, 1934.) 



Oros. per 100 gna. sat. sol. 



HgClg 


HgBr 2 


31.35 


0.0 


31.0 


3-3 


27-3 


7.1 


25.8 
26.0 


9.8 

10.0 


24.0 


12.2 


22.2 


14.1 



Percent HgBr,. 
in Solid Phaae 



27 



Qms. per 100 ^gma. sat, sol. 



HgCl 2 


HgB: 


P 2 


17.4 


20. 


5 


14.0 


22. 


4 


10.7 


21. 


8 


10.4 


22. 


i 


6.7 


24. 


6 


3.8 


20. 


2 


0.0 


18. 


1 



Percent HgBr g 
In Solid Phase 

50 
60 



100 
100 



Br 



The solid phase consists of a. series of mixed crystals up to about 
70 percent HgBr 2 . 

SOLUBILITY OF MERCURIC BROMIDE IN ETHYL ALCOHOL SOLUTIONS 
OP POTASSIUM BROMIDE AT 3/1 AND VICE VERSA. 

(Pernot, 1933.) 

The original results are given only in the form of diagrams from which 
the following approximate figures have been read. 



Results for Absolute C 2 H g OH 

Qms. perlOOams. sar,. sol. Solid 

* ' Phase 



Results for 95 Percent CJi OH 



HgBr 


K3r 


2 




25.0 


0.0 


35-0 


3-0 


40.0 


4-5 


45.0 


6.0 


40.0 


6.0 


25.0 


6.0 


20 


6.0 


20 


7.0 


15 


5.5 


10 


4-0 


5 


2.0 



" + KBr 
KBr 



1.1. A = HgBr 2 .KBr.C 2 l! 5 OH 



Gms. per 100 g 


jns. sat. sol. 

" Icir" 


Solid 
v Phase 


HgBr 2 


19.0 
30.0 
40.0 


0.0 
3.0 

6.0 


HgBr 2 

tl 


45*5 


7.2 


" + i.: 


35.0 
30.0 


7.2 

7.5 


1.1. H 
ti 


25-5 
28.0 


8.5 

12.0 


it 


30.5 
20.5 


14.5 
10.0 


11 + KB 
KBr 


10.0 


5.0 




1.1. H = 


HgBr 2 .KBr. 


H 2 



HYDRARGYRUM 6lO 

SOLUBILITY OF MERCURIC BROMIDE IN AN EQUIMOLECULAR MIXTURE OF 
ETHYL ALCOHOL AND BENZENE. (Dukeiski, 1907.) 

t- o. 10. 20. 30. 40. 50. 60. 

Gms. HgBr 2 per 100 Gms. Sat. Sol. 10.7 12 14 16 17.5 19 21 
loo gins, of sat. sol. in acetone at 25 contain 34.76 gms. HgBr2. 



SOLUBILITY OF MERCURIC BROMIDE IN ANILINE. 



(Reinders, 1900.) 
(Staronka, 1910.) 



Gms. 



Solid Phase. 



Gms. 

:r 

Hi 

" *fHgBr 4 .QH s NH, 
HgBr,.C,H,NH, 



100 gms. ethyl acetate dissolve 13.05 gms. HgBr 2 at 18. (Naumann, 1910.) 

100 gms. methyl acetate dissolve 21.93 gms. HgBr 2 at 18 (d^ sat. sol. = 1.090). 

(Nuumann, 1909.) 

SOLUBILITY op MBRCURIC BROMIDE IN ANHYDROUS ACETIC ACID 
DETERMINED BY THE SYNTHETIC METHOD. 

(Davidson and Chappeil, 1938.) 



r. 


Mol. % 
HgBr 2 . 


?4 B Gm Solid Phase. f. 


Mol. % 
HgBr,. 


HgBr 2 p 
100 Gm 






C 6 H 6 NHj. 




QH 6 NH 


60 


4 


16.14 HgBrj.aCeHjNHj Iio* 


A 33.3 


193.3 


70 


5-8 


23.83 


109. 


7T 33-5 


195 


80 


8-3 


35.04 


IIS 


37.2 


229.3 


90 


12.2 


53.8o 


120 


42.3 


283.8 


100 


18.8 


89.64 


124 


50 


387.2 


*5 


23.2 


116.9 ' 123 


55-4 


480.9 






* M. pt. t 


Eutec. 





t o 


Mola. HgBr per 


Solid 




t o 


MolS. 


HgBr per 100 Solid 




100 


raols. HgBr 2 * CH 3 COOH 


Phase 




c 


100 mols. HgBr '* CH^COOH Phase 


16.5 






0. 194 




CH.COOH 




75 







.707 Hg 


Br 


25 






0.261 




Hgr ? 




86 







.860 


11 


32 






0.287 




H 




92 







.998 


M 


41 






0.350 




" 




97 




1 


13 


" 


51 






0.413 


103 


1 


.29 


11 


58 






0.477 


" 110 


1 


50 


11 


71 






0.650 


















SOLUBILITY OF 


MERCURIC BROMIDE IN PYRIDINE. 


(Staronka, 1910.) 










Gms. 










Gms. 








t. 


Mol. % 
HgBr 2 . 


HgBr 2 per 
100 Gms. 


Solid Phase. f Mol % HgBr, per 
UK>V. HgBrj. 100 Gms. 


Solid Phase. 










C 6 HN. 










C 6 H,N. 








10 


5 




24 


HgBrj.aCjHjN 107 


* 


39 


291 . 5 HgBr,.2C 8 H,N+HgBr 2 .C 6 H 4 N 


30 


8 




39-^4 




no 


40.4 309 


HgBr 2 .C,H 5 N 




50 


II. 


2 


57-49 




120 




45 


5 38L3 




'* 




80 


17. 


5 


96.68 


I23f 50 


455-8 




" 




100 


22 




128.5 




125 




51 


474-4 




3HgBr 2 .2C ft H|N 




no 


24. 


5 


147.8 




130 




54 


-2 539.4 




" 




ii8f 


33- 


3 


227.6 




134 


t 


60 


683.7 




" 




no 


35- 


5 


250.8 




133 




64 


810.4 



















* Eutec. 


1 


fin. 


pt. 








SOLUBILITY OF MERCURIC BROMIDE 


IN 


QUINOLINE. 




(Staronka, 1910.) 










f. 


Mol. % 
HgBr 2 . 


Gms. HgBr per 
100 Gms. CsHvN. 


Solid Phase. 








88 


4-4 


12. 


85 


HgBr 2 . 2 C 9 H 7 N 








in 


8. 9 


27. 


28 




u 














127 


14-3 


46. 


58 




it 














134 


I 7 .6 


61. 


16 




tt 









Data for the solubility of mercuric bromide in nitrobenzene, in p nitrotoluene, 
in m nitrotoluene, in o nitrotoiuene 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 HgBr 2 + Se are given by Olivari, 1912. 



6n HYDRARGYRUM Eg 

DISTRIBUTION OF MERCURIC BROMIDE BETWEEN WATER AND BENZENE 
(THIOPHENE FREE) AT 25. (Sherriil, 1903.) 

Mob, per Liter. Mob, per Liter. ^ Coef 

H,0 Layer. QHe Layer. "". &0 Layer. CHe Layer. 

0.017 O.IQ4 0.876 0.00634 0.0715 0.59 

0.01147 0.1303 0.88 0.003.94 0.0436 0.90 

0.00953 0.1074 0.89 0.00320 0.0353 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 HgBr s + HgI 2 in acetone at 25 and 
in ethyl alcohol of & = 0.8126 = 95% at o, 25 and 50 are given by Remders 
(1900). In the case of acetone, the ratio of HgBr 2 in the solution increases with 
increase of per cent of HgBr 2 in the solid phase. In the case of the alcohol solu- 
tions the ratio in solution does not show such regular variations with change ot 
per cent of MgBr2 in the solid phase. 

SOLUBILITY OF MERCURIC BROMIDE IN ORGANIC SOLVENTS. g r 

In Carbon Disulfide. In Other Solvents at i8-20. 

(Arctowski, 1894.) (Sulc., 1900.) 

Cms. Hg B r 2 Gins. HgBr t Gms. HgBr t 

t. per 100 Cms. t. per roo Gms. Solvent. Formula. per 100 Gms. 

Solution. Solution. Solvent. 

io 0.049 I 5 0.140 Chloroform CHCls 0.126 

5 0.068 20 0.187 Bromoform CHBr 3 0.679 
o 0.087 25 0.232 Carbon Tetrachloride CCU 0.003 

+ 5 0.105 3 0.274 Ethyl Bromide C2H 5 Br 2.31 

io 0.122 Ethylene Dibromide C 2 H 4 B r 2 2.34 

One liter benzene dissolves 6.99 gms. HgBr 2 at 25. (Abegg and Sherriil, lyoj.J 

100 pros. sat. solution of Mercuric Bromide in Acetone contain 33.9 
gms. HqBr 2 at 25. (Zapata y Zapata, 1930.) 

100 Rms. of liquid Sulfur Dioxide dissolve 0.074 gro- HgBr g at o 



oxe ssove 0.074 g- 

(Jander and Ruppolt, 1937.) 



Fusion-point data have been determined for the following mixtures". 



HgCl 2 (Losana, 1926.) 

HgI 2 

" * HgCl 2 

HgSO (Paic, 1930, 1933.) T 

AgNO 'Bergman, 1922-24, 1926; Bergman, Genke and Isaikin, 

" " " 1922-2^.1 



HgBr p 



T1S0 4 (Woskresenskaja, 1929.) 

PbBr (Sandonnini, 1912, 1924.) ^ ^ 

2 BrO 

MERCURY BROMATE (ic) normal Hg(Br0 3 ) s , basic HgOHBrO 3 . 

SOLUBILITY OF EACH IN AQUEOUS SOLUTIONS OF PERCHLORIC ACID AND OF 
NITRIC ACID AT 45. ( Smith, 1924. ) 

Results for Hg(Br0 3 )a Aq : Results for HgOHBrG 3 in Aq : 

Perchloric Acid. Nitric Acid. Perchloric Acid. Nitric Acid. 

Gms. Gins. Gms. Gms. 

Approx. Hg(lirOj), Approx. irg|DrO a ) s Approx. IlffOHBrOg Approx. HgOIIBrO, 

Normality per 100 cc. Normality per 100 ce. Normality per 100 cc. Normality periOOcc. 

of IIC10 4 . sat. sol. of IIXO a . sat. sol. of IICIO',. stil. sol. of HN0 3 . sut. sol. 

2.0 6.58 2.0 14.66 o.o(=H 2 0) 0.081 i.o 12. 52 

>..5 5.2A 3.o i5.oo i.o 4.34 5.-0 ai.So 

3.o 4.i3 4.0 14.99 2 - 5 -94 

3.5 3.4o 5.o 14.75 a. 5 6.06 

4.0 2.58 3.o 6.06 

5.o i.55 



Hg HYDRARGYRUM 6l2 

MEBCURY ACETATE fous) Hg 2 (CH 3 COO) 2 . 

SOLUBILITY OF MERCUROUS ACETATE IN WATER AND IN AQUEOUS ACETIC ACID 

AT C 2l. (Legerlotz, 1918.) 

Recryslallized mercurous acetate was rubbed with water or aqueous acetic 
acid uritill thoroughly wet and the mixture constantly shaken in a thermostat 
for 120 hours. The saturated solution was analyzed by adding a slight excess 
of Na Ci to precipitate Hg Cl and this latter filtered, dried and weighed. 

Gros. Hg, ( CII, COO I 2 
Solvent. per 100 cc. sat. sol. 

Water o. 1024 

Aq. acetic acid (cone. = 2j 0.0730 

(cone. = 4) 0.0690 

(cone. = 6) o.o65o 

The amount of acetic acid corresponding to cone. 2, 4 and 6 is not stated. 

100 gnis. sat. solution of Mercurous Acetate in Water contain 0.75 
gm. Hg 2 (CH C00) 2 at 13. (Welsh and Broderson, 1915.) 

The Solubility Product of Hg 2 (CH CQO) 2 in Water at 25 is 2.0 x io" 16 
(Bargarsky 1897, reported by Brodsky, 1929.) 

loocc anhydrous Hydrazine dissolve about 2.0 gms. Hg 2 (CH 3 COO) 2 at 
about 20 with precipitation of Hg. (Welsh and Broderson, 1915.) 

100 gms. Methyl Alcohol dissolve 1.24 gm. Hg 2 (CH 3 COO) 2 at 15 and 
i. no gm. at the b. pt. (66.3). (Henstock, 1934.) 
HYDRARGYRUM ACETATE (Mercuric Acetate) Hg (CH 3 COO) 2 

100 gms. water dissolve 25 gms. Hg(CH 3 COO) 2 at 10. (Welsh and 

Broderson, 1915.) 

100 gms. Methyl Alcohol dissolve 7.5n gms. Hg(CH C00) 2 at 15 and 

49.84 gros. at the b. pt.(66.7). (Henstock, 1934.) 

100 gms. Acetone dissolve 0.60 gm. Hg(CH 3 COO) 2 at 15. (Henstock, 

1934- ) 

100 grcs. of liquid Sulfur Dioxide dissolve 0.095 g m N? (CH 3 COO) g 
at o. (Jander and Ruppolt, 1937.) 
SOLUBILITY OF MERCURIC ACETATE IN MIXTURES OF PHENOL AND ACETIC ACID 

AT lo. (Mameli and Cocconi, 1922. } 
Cms, per 100 gws. sat. sol. dins, per 100 #ms. sal. sol. 

"iisfcn a r.ooi,. <: r ,H s oir. cn 3 coorr. 'i7gi(:H 3 cooT 1 "' c 8 H 6 on. nr 3 cooH. 

34.o3 51.93 14.04 35.46 59.. 82 11,7?. 

4o.o8 5i.()o 8.02 8.61 i8.65 72.74 

7.40 8.40 84.20 9.28 34-99 55.78 

42.02 52.20 5.78 i3.56 43.76 4'2.68 

9.65 19.46 70.89 ->.8.53 50.76 20.71 

Data for the f. pt. of Hg (CH 3 CO 0) 2 + C a H 5 OH and other mixtures are also 
given by Mameli and Cocconi. 
MERCUROUS TARTRATE 



The Solubility Product of Mercurous Tartrate in Water at J8, as 
quoted from Behrend, 1894, by Rrodsky, 1929, is (2).io~ 10 . 

MERCURY NitrosoPHENYL Hydroxylamine HgC 6 H g .N(NO) 0] . 

This compound is prepared by precipitating in acid solutions, salts 
of mercury with "Cupferron" (the ammonium salt of nitroso phenyl 
hydroxylamine). Its solubility in water at 18 is less than 1.3 x io 
gm. atoms or 0.3 mg per liter. (Pinkus and Martin, 1927.) 



613 HYDRARGYRUM H 

MERCURY BENZOATE (ic) IIg(C 6 H 5 COO ),.H 2 0. 

100 cc, of sat. sol. of mercuric benzoate in water contain 0.209 gm. Hg (C 6 H 5 COO) a 

at 20 o ( Ephraim and Pfister, 1925v j 

100 gms. H g O dissolve 1.2 gm. Hg(C e H g COO) 2 at 15 and 2.5 gms. at 
100. (Tarugi and Checchi, 1901.) 

100 gms. Methyl Alcohol dissolve 3.67 gms. Hg(C fl H C00) 2 at 15 and 
3.67 at the b. pt. (66.5). 100 gms. Acetone dissolve 7.23 pis. 
Hg(C 6 H g COO) 2 at 15. (Henstock, 1934-) 

100 gms. Benzene (C 6 H 6 ) dissolve 2.49 gms. Hg(C 6 H 5 COO) 2 at 15. 
(Henstock, 1934.) 

MERCURY CINNAMATE (ic) (C 6 H 6 CH.CHCOO) 2 Hg.?H 2 O. 

100 gms. HaO dissolve about 0.03 gm. mercuric cinnamate at 25. (De Jong, 1906.) 
loogms. H20 dissolve about o. 53 gm. Hg cinnamateat 100. (Tarugi &Checchi, 1901,) 

MERCURY DiPHENYL Hg(C 6 H g ) 2 . 

Fusion-point data for mixtures of H&(C fl H 5 ) g * Sn(C fi H g ) 4 and for 
Hg(C Q H 5 ) 2 # Sb(C fi H 5 ) 3 are given by Cambi, 1912. 

MERCURIC Diazoamino BENZENE Hg(C 6 H 5 N = N-C fl H 5 ) g . 
SOLUBILITY IN ALCOHOLS. 

(Watt and Fernellua. 1935.) 

Oms. Hg(C 6 H s N=N-C 6 H 5 ) 2 
Alcohol t p^p liter sat. sol. 

Methyl Alcohol 25 0.0116 

Ethyl Alcohol 25 0.0052 

n Propyl Alcohol 25 0.0228 

MERCURIC CAMPHOR CARBONATE Hg (C 1Q H 15 O.C0 2 ) g 
SOLUBILITY IN SEVERAL SOLVENTS. 

(Picon, 1931.) 

This compound is made by allowing camphoric acid and yellow oxide 
of mercury to react in the cold in presence of a small amount of water. 

ana. Hg ( c 10 H ls o.co 2 ) 2 
Solvent t per llter sat> 80U 

Methyl Alcohol 15 44-9 

Ethyl Alcohol 10 46.0 

Ethyl Ether 10 133-0 

Acetone 12.5 8^.7 

Ethyl Acetate 12.5 82.6 

Chloroform 12.5 3?6.2 

Carbon Tetrachloride 12.5 215.9 

Benzene 15.0 560.3 

Carbon Disulfide 15 341-25 

Petroleum Ether 10 43-4 

Gasoline 10 145.2 

Oil 15 50.0 



HYDRARGYRUM 614 

HYDRARGYRUM (Mercuric Palnitate and Stearate) 

SOLUBILITY OP EACH SEPARATELY IN SEVERAL SOLVENTS AT 20. 

(Dletzel and Sedlneyer, 1928.) 

Weighed amounts of compound and solvent were shaken for 30 hours. 
The mixture was the filtered and the excess of undissolved compound 
weighed and the amount dissolved found by difference. 

Results for H$> Palmitate Results for Hg Stearate 



solvent 0| - Mols - Hg t C ie H 3l2 ) 2 Solvent . *' M l8 * ^leSsV 2 

S 1VenC per liter sau JJl? * * "w sat - <* 

Abs. Bthyl Alcohol 0.0005*04 Abs. Ethyl Alcohol 0.0006809 

Ethyl Ether 0.0005460 Ethyl Ether 0.0005061 

Chloroform 0.0007627 Chloroform 0.0007279 
Mixture of Alcohol Mixture of Alcohol 
Chloroform & Pyridine 0.01261 Chloroform & Pyridine 0.001380 



MERCURY FULMINATE C 2 HgN 2 2 . 

One liter of solution in water contains 0.70 gm. C 2 HgN 2 O 2 at 12 and 1.76 

gms. at 49. (Holleman. 1896.) 



CN MERCURIC CYANIDE Hg(CN) 2 . 

SOLUBILITY IN WATER. 

f Gms.Hg(CN) 2 perioo: Authority. 

Gms. H 2 O. cc. Sat. Sol. 

o.45Eutec. about n ... (Guthric, 1878.) 

13.5 9.3 ... (Timofeiew, 1894.) 

15 12. 5 ... (Marsh and Struthers, 1905.) 

20 9.3 (Konowalow, 1898, 1899.) 

25 ... 11.12 (Sbcrrill, 1903.) 

25 11.27 IO. 95 (^=1.0813) (Herz and Anders, 1907.) 

101 . 1 S3-85 ... (Griffiths.) 



The Solubility Product of Mercuric Cyanide in Water at 25 is 
5.0 x io" 40 as calculated from the results of Immerv^ahr by Brodsky, 
1929. The following results for the Solubility of Mercuric Cyanide 
in Water at temperatures above 100 are given by Benrath, Gjedebo, 
Schlffers and Wunderlich, 1937. 



Gms. Hg(CN) 2 per 100 gms. sat. sol. 35.8 42.9 49.8 56.7 63.4 72.8 



615 HYDRARGYRUM 

SOLUBILITY OF MERCURIC CYANIDE IN AQUEOUS POTASSIUM CYANIDE SOLU- 

TIONS AT 25. (Shcrrill, 1903.) 
Mols per Liter. Cms, per Liter. 

" " 



Hg 



0.0493 
0.0985 
0.1970 



Hg(CN) 2 : 
0.4855 
0.5350 
0.6270 



Hg(CN) 2 . 
122.6 



3.21 

6.41 135.2 

12.83 158.4 

The regularity of the increase in solubility proves that the complex Hg(CN)i. 
KCN is formed at the given concentrations. 

Data are also given for the distribution of Hg(CN) 2 between aqueous solu- 
tions of KCN and ether at 25. 

HYDRARGYRUM CYANIDE (Mercuric Cyanide) 

SOLUBILITY OP MERCURIC CYANIDB IN AQUBOUS SOLUTIONS o? 
POTASSIUM CYANIDB AT 25 AND VICE VERSA. 

(Corbet, 1936.) 

Due to the difficulty of preparing KCN free from KOH the saturated 
solutions were prepared from double salts which were free of KOfl. 
The solutions were kept in contact with an atmosphere of coal gas 
previously washed by being passed through solutions of lead acetate 
and NaOll. 



Gms. per 100 gms. sat. sol. 


! 


i mm 


Solid. 


KCN. 


Hg(CN) 2 . 


Phase. 


4L7 


0.00 


KCN 


39.7 


o.49 


KCN-t-KjHg(CN), 


29-47 


2.34 


K,Hg(CN)* 


17. 34 


11.09 





14.54 


i5.54 


,) 


11.54 


20.65 





12.51 


SLID 





*Shorrill, Z 


'. Physik Chem 


., 43, 719, i 9 o3. 



Urns/ per 100 gins. sat. sol. 


Solid. 


KCN. 


11* (CN),. 


Phase. 


12. 8l 
I1.3 7 


39.96 

4i.85 


K s Hg(CN) 4 
H ff (CN), 


3-97 


20.34 





* I .09 


i8.53 





*o.56 


u.83 





*o.a8 


10.89 





*o.oo 


10.00 






CN 



MERCURY CYANIDE ( ic) Hg(CN) a . 

SOLUBILITY OF MERCURIC CYANIDE IN AQUEOUS SOLUTIONS OF AMMONIA AT 0. 

(Brinkley, 1922). 

Cms. per 100 gms. sat. sol. Gms. per .100 gms. sat. sol. 



6.3i 


NH,. 
O.O 


Solid Phase. 

Hg(CN), 


Wg(CN),. 
24.68 


Nir 3 . Solid Phase. 

9.40 Hg(CN),.NH, 


8.46 


0.43 





25.41 


9.55 


H-HlCK) 9 .! 


11.66 


1.09 


-f-irg(CN) s .NII 3 


24 o4 


u.23 Hg 


r (CN')j.'2 NH 


9.40 


2.06 


Hg(CN) s .NH 3 


23.40 


12.59 


)) 


I . 32 


4.08 


)) 


24.46 


16.87 


)) 


15.43 


6.82 


)) 


43.57 


22 . 09 





17.51 


7-67 





66. i o 


> | < 5 j 


V 


19. 3i 


8.25 





79 .3o 


20 . 70 






One liter 5.2% aqueous NH 3 solution dissolves 204.3 gms. Hg(CN) 2 at about 20. 

(I\ono\valo\v, 1898.) 



HYDRARGYRUM 616 

SOLUBILITY OF MERCURIC CYANIDR IN AQUEOUS SOLUTIONS OP 
POTASSIUM SODIUM TARTRATB AND OF SODIUM ACBTATE AT 18-20. 

(Bordelanu* 1333.) 
In aqueous solutions of: 



Gtoa. per 100 ( 


5ms. sat* sol. 


KKac 4 H 4 o e 


Hg(CN)g 


7.5 
10.0 
15.0 


9.6s 
9.69 
10.38 


-20,0 


10.73 





NaCH.COO 

o 


Qtos. per 


100 0ns. sac. sol. 


NaCHjCOO 


Hg(CN) 2 * 


8.84 
16.57 
32.52 


9.11 
9-40 
9.69 



CN 



SOLUBILITY OF MERCURIC CYANIDE IN AQUEOUS SOLUTIONS OF METHYL ALCOHOL, 
ETHYL ALCOHOL AND OF ETHYL ACETATE AT 25. (Herz and Anders, 1907.) 

In Aq. Methyl Alcohol. In Aq. Ethyl Alcohol. In Aq. Ethyl Acetate. 



\Vt. % 
CH,OH in 
Solvent. 


Sat. Sol. 


urns. 
Hg(CN), 
per loo cc. 
Sat. Sol 


Wt. % 
QH 5 OH in 
Solvent. 


Sat. Sol. I 


urns. 
>er 100 cc. 


Wt. % 


6 Sat. Sol. 


urns. 
H*(CN), 
oerioocc. 
Sat. Sol. 


IO.6 


I 


.0640 


11.02 







1.0813 


10.95 


o 


I . 


,0810 


10.95 


30-77 


I 


.0484 


12.46 


2O. 


18 


1-0339 


8.76 


4.39 


I. 


0798 


10.83 


47.06 


I 


.0426 


16.37 


40. 


69 


I. 0006 


9.02 


96.76 


I. 


9374 


2.66 


64 


I 


.0441 


20.48 


70. 


.01 


0.9419 


9-57 


100 


O, 


9097 


1. 80 


78.05 


I 


.0484 


24.58 


100 




0.8552 


8.19 










100 


I 


.0762 


34> 2 9 



















SOLUBILITY OF MERCURIC CYANIDE IN ETHYL ALCOHOL, METHYL ALCOHOL 
AND IN MIXTURES OF THE Two. 



i Ethyl Alcohol. 

Gms. Hg(CN) 2 
t. per roo Gms. 


In Methyl Alcohol. 

(Dukelski, 1907.) 

Gms. Hg(CN) 2 
t. per too Gms. 


In CHaOH-f C 2 H 6 OH at 25. 

(Hera and Kuhn, 1908.) 

% CH 3 OrI d of Gms. Hg(CN), 
in _"-.. ner 100 cc. 




Sat. Sol. 




Sat. Sol. 


Mixture. 


bat. bol. 


Sat. Sol. 


O 


8-3 


O 


26.10 


4-37 


0.8618 


9.02 


10 


8.8 


14.17 


29.17 


10.4 


0.8707 


10.10 


20 


9-25 


23-4 


32.01 


41.02 


0.9267 


16.70 


25 


9-53* 


27.4 


31-77 


80.69 


1.024 


28. 20 


30 


9-8 


31-7 


32.53 


84.77 


1-034 


29.60 


40 


10.3 


38.1 


33-29 


01.25 


1.052 


30 


*rfj 


^=0.8552 


44-5 


34-05 


ICO 


1.076 


34-30 



loo gms. of a sat. solution of Hg(CN)2 in a mixture of equimolecutar amounts 
of CHjOH and C 6 He contain 10.2 gms. Hg(CN) 2 at 10, 13 gms. at 30 and 15 
gms. at 50. (Dukelski, 1907} 



100 gms. Methyl Alcohol dissolve 34.55 gms. Hg(CN) 
59.84 gms. at the b. pt. (67). 
" 100 gms. Acetone dissolve 10.3 gms. Hg(CN) 2 at 15. 



at 15 and 

(Henstock, 
1934.) 



6i 7 



HYDRARGYRUM Hg 



SOLUBILITY OF MERCURIC CYANIDE IN MIXTURES OF PROPYL AND METHYL 
ALCOHOLS AND PROPYL AND ETHYL ALCOHOLS AT 25. (lien and Kuhn, 1908.) 



In C 3 H 7 OH+CH 8 OU. 



In CnH 7 OIH-C 2 H 8 OH. 



in Mixed 
Solv<* nf 


ic j r Gms. f.//"UAr 
^of rf^of H g(CN) 2 ^$* 
Solvent. Sat. Sol. per 100 cc. ^L^r 


Solvent. 


, f Gms. 
rf -V of Hg(CN) 2 
Sat. Sol. per 100 cc. 








Sat. 


Sol. 












Sat 


. Sol. 







0.7878 1.0760 


34- 


3 


o 





.7867 


O 


.8552 


8 


.91 


II. 


II 


0.7894 1.0327 


29. 


52 


8.1 





.7886 


O 


.8549 


7 


.90 


23- 


80 


0.7907 0.9891 


24. 


48 


17-85 





.7902 


O 


.8527 


7 


30 


65- 


20 


0.7954 0.8800 


10. 


48 


56.6 


o 


.7926 





.8386 


5 


.21 




80 


0.7992 0.8376 


5. 


04 


88.6 





7973 


O 


.8311 


3 


.87 


93- 


75 


0-7995 -8335 


4- 


23 


91.2 





7979 


O 


.8306 


3 




96. 


60 


0.7999 0.8322 


3- 


.98 


95-2 


o 


.7986 


O 


.8293 


3 


64 


IOO 




0.8004 0.8283 


3- 


44 


IOO 


o 


.8004 





.8283 


3 


.44 


IOO 
IOO 


gms. 
gms. 


propyl alcohol dissolve 3, 
'acetonitrile (b. pt. 81.6) 


.79 gms. Hg(CN) 2 
dissolve 9.58 gms. 


at 13.5. 

Hg(CN) 2 


(Timofeiew, 
at 1 8. 


1894.) 

-*.- . ^ 



(Naumann and Schier, 1914.) 

loo gms. benzonitrile' (b. pt. 190-1) dissolve 1.093 gms. Hg(CN) 2 at 18. 

(Naumann, i9jf4j) 

SOLUBILITY OF MERCURIC CYANIDE IN ANILINE. (Staronka, 1910.) 

t of Solidification 41 49 58.5 65 77 83.5 84 88.5 

Mol.%Hg(CN) 2 insat. 
Solution 3.7 5.7 7.7 9 14.2 18.2 19.7 23.4 

The solid phases are the unstable Hg(CN) 2 .4C 6 H 6 NH 2 and the stable Hg(CN) 2 . 
2C 6 Hj>NH 2 (m. pt. about 90). 

One liter sat. solution in ethyl ether contains 2.53 gms. Hg(CN)a at 25. 

(Abegg and Shorrill, 190.1 ) 

loo gms. glycerol dissolve 27 grns. Hg(CN) 2 at 15.5. 

SOLUBILITIES OF MERCURIC CYANIDE DOUBLE SALTS IN WATER AND 

IN ALCOHOL. 



Double Salt. 



cold 



Hg(CN) 2 .2KCN 

Hg(CN) 2 .2TlCN i 

Hg(CN) 2 . 2 TlCN 10 
2Hg(CN) 2 .CaBr 2 . 5 H 2 O cold 
2Hg(CN) 2 .CaBr 2 . 5 H 2 O boiling 

Hg(CN) 2 .KCl.H 2 O 18 

Hg(CN) 2 .KBr. 2 H 2 O 18 

Hg(CN) 2 . KB r. 2H,O boiling 

Hg(CN) 2 .BaI 2 . 4 H 2 O cold 

Hg(CN) 2 .BaI 2 . 4 H.,O boiling 

Hg(CN)o.KI cold 

Hg(CN) 2 .NaI.2H 2 O 18 

Hg(CN) 2 .SrI 2 .6H 2 O 18 



Gms. per TOO Grams. 
\Vater. Alcohol. ' 

22.7 

12.6 

9.7 

IOO.O 



400.0 

14.81 

7-49 

IOO.O + 

6.42 

250.0 

6.2 
22.2 



50.O 
IOO.O 



Observer. 

(Fromuller Ber. n, pa, '18.) 
I* 

(Custer.) 
(Brett.) 



4.42 (Custer.) 

62*5 (90% Ale.) 

1. 04 (34 B Ak.) (Caillot.) 

15.4 (90% Ale.) (Custer.) 

25.0 (90% Ale.) 



xoo Gms. 
O.005 
O-OOI 
0.013 
O-OOI 



14-3 

SOLDIULITY OF MECUR1C CYANIDE IN ORGANIC SOLVENTS AT 1 8~2O. 

(Sulc. 1900 > 

Solvent. Formula. 

Bromoform CHBr 3 

Carbon Tetra Chloride CC1 4 

Ethyl Bromide C 2 H 5 Br 

Ethylene Di Bromide C 2 H 4 Br 2 

Data for the ternary system, mercuric cyanide, phenol, water are given b>- 
Timmermans, 1907. 



CN 



6i8 



Hg HYDRARGYRUM 

SOLUBILITY OF MERCURIC CYANIDE IN PYRIDINE. (Staronka, 1910.) 

Mols. 
1* 

Solid Phase. 



CN 



Mois. 
Hg(CN) 2 
. penooMols. Solid Phase. 



t. per 100 





*H 


[g(CI 


sT) 2 -f 




H 


ftS 


Or 


-C S H 6 N 


C 8 H 6 N 


9 




7. 


, I Hg 


(C^j.eCsHsN" 22. 


5 


17 


3 


ii 




8, 


7 


28.5 


18 


4 


12. 


.2 


10. 


4 


32 




19 


3 


13 




ii. 


3 


38 




20 


.6 


13 


5 


12, 




42 




22 


3 


1.4- 


5 


13 


.8 


46 




23 


7 


16. 


5 


15 


.8 


53 




25 


-3 


20.5 


15 


-9 


54 


5 


26 





Mols. 

er 100 Mols. Solid Phase. 
-f 



tr. per 100 J\ 

*& 

56.5 26*6 2Hg(CN) s . 3 CsHN 
68 27.5 
70 27.7 



86 
in 
122.5 
125 
141 



29 

32 * 
33-8 

34-4 
3^.3 



100 gms. pyridine dissolve 64.8 gms. Hg(CN) 2 at 18. 



(Schroeder, 1905.) 



SOLUBILITY OF MERCURIC CYANIDE IN QUINOLINE. (Suronka, 1910.) 



Mols. Hg(CN) 2 

f. per roo Mols. Solid Phase. t. 

Hg(CN) 2 +C 9 H 7 K. 

45 4-2 Hg(CN) 2 . 3 C,H 7 N 137 

54 6 *' tr. pt. 60 161 

89 (61) 8.2 180 

99 (61) 9.2 192 



Mols. Hg(CN) 2 

per loo Mols. Solid Phase. 

Hg(CN) 2 4-C,H 7 N. 

13.2 Hg(CN),.2CH 1 N(?) 

17.4 

22. S 

2 7 .! 



CNS 



100 Rms. liquid Sulfur Dioxide dissolve 0.014 gm. Hg(CN) g at o. 
(Jander and Ruppolt, 1937.) 



MERCURY Oxy CYANIDE HgO.Hg(CN) 



2 . 



SOLUBILITY OP MKRCURY OXY CYANIDE IN AQUBOUS SOLUTIONS AT 18-20 
(Bordalanu, 1933.) 

In aqueous solutions of: 



Oms. per 100 jpns. sac, sol. 
HgO.Hg(CN) 2 ~ 

l.bO 
1.94 
2.00 
2.18 



The author also gives results showing that the presence of 
has little effect upon the above solubilities. 



KNaC 4 H 4 


e-* R 2 




NaCH 3 COO 




us. per 100 gr 


is. sac. sol. 


Ons. per 


100 gms. sac. sol. 


Qms. 


* C 4 H 4e 


HgO.Hg(CN) 2 N 


'NaCH 3 COO 


HgO.Hg(CN) 2 N 


'H 3 B0 3 


o.o 

12.0 
20.0 


1.315 
3.18 
4-39 


8.25 

18.74 
35.72 


1.291 
1.170 
1.063 


0.4 
1.4 
2.4 


42.O 


5.73 






3-4 



MERCUROUS THIOCYANATE H 

The Solubility Product of Mercurous Thiocyanate in Water at 25 is 
3.0 x 10"* as quoted by Brodsky, 1929 from Immerwahr/and 1.4 x io" 20 
as quoted from Grossmann, 1905. 



619 HYDRARGYRUM Hg 

MERCURIC THIOCYANATE Hg(SCN 2 fe 

EQUILIBRIUM IN THE SYSTEM MERCURIC THIOCYANATE, POTASSIUM 
THIOCYANATR AND WATER AT 25. 

(Mason and Forgeng, 1931,) 
The authors determined the following triple points of the system: 

Oms. per IQO^gms. sat, sol. Solid 

KSCN Hg(SCN)~ ^ Phase 

o.o 0.063 Hg(SCN) 

2.05 4.05 " + KHg(SCN) 

33.1 49.1 K 2 Hg(SCN) * " 

66.4 10.4 " * KSCN CNS 

70.5 o.o KSCN 

MERCURIC THIOCYANATE 

100 tns. liquid Sulfur Dioxide dissolve 0.02 gm. Hg(SCN) 2 at o. 
(Jander and Ruppolt, 1937.) 

MERCURIC Zinc THIOCYANATE HgZn(SCN) 4 - 

SOLUBILITY OF MERCURIC ZINC THIOCYANATE IN AQUEOUS 
SOLUTIONS OF AMMONIUM CHLORIDE. 

(Cuveller, 1935.) 

Measured amounts of aqueous solutions of HgNa 2 (SCN) 4 , Zn(N0 3 ) ? , Cu(SCN^ 
and MH Cl of known concentration were mixed and the amount of zinc not 
precipitated as HgZn(CNS) g was determined by a colorimetric comparison. 

Thus the amount of HgZN(SCN) 4 remaining in solution at each concentra- 
tion of NH 4 C1 was estimated by difference. 

Normality Oms. HgZn(SCN) 4 Normality Ofcs. HgZn(8CN) 4 

of Aq. NH Cl Per 100 gms. sat. sol. of Aq. NH^Cl per 100 gms. sat. sol. 

0.022 0.0766 0.714 0.462 

0.044 0.110 1.000 0.505 

0.089 0.173 l -428 0.534 

0.178 0.255 1.843 0.546 

0.357 0.353 

MERCUROUS CARBONATE Hg g C0 3 

The Solubility Product of mercurous carbonate in water at 25 is 
9.0 x io" 17 as quoted from Immerwahr by Rrodsky, 1929. 

COO 

MERCUROUS OXALATE HggC^ 

The Solubility Product of mercurous oxalate in water at 25 is 
(2).x io" 13 as quoted from Ben rend by Brodsky, 1929. 

MERCURIC OXALATE %C 2 4 . 

100 gms. H 2 dissolve 0.0107 gm. HgC 2 A at 20. (Trifnov, 1024, 1925.) 

Data for the system. HgG 2 4 -i- K 2 G 2 4 + H 2 O atao are also g;iven. The five 
branches of the curve have, respectively, for solid phase : rIgC.>O 4 ; K 2 Go O^HgCnO* 
.2H 2 0, ftK a C 1 4 .HgC 2 1 .3H 2 0, 3K,G,0 4 .HgG 2 04.4H 2 O~ and K a C a O*. 



Hg HYDRARGYRUM 620 

MERCUROUS CHLORIDE Hg 2 Cl 2 

SOLUBILITY OF MERCUROUS CHLORIDE IN WATER. 

Gms. Hg,Cl 2 Gms. Hg 2 Cl 2 

t. per 100 Gms. Authority. t. per 100 Gms. Authority. 

Sat. Sol. Sat. Sol. 

0.5 O.OOOI4O (Conductivity, Kohlrausch, 1908.) 24.6 O.OOO28 (Kohlrausch, 1908.) 

l8 O.OOOO75 (Indirect, Behrend, 1893.) 25 O.OOOO47 (Sherrill, 1903.) 

1 8 O.OOO2I (Conductivity, Kohlrausch, 1908.) 43 0. 00070 (Kohlrausch, 1908.) 

2O O.OOOOjS (Ley and Heimbucher, 1904.) 

The solubility product of mercurous chloride, determined by a modified electro- 
metric method, was found by Brodsky and Scherschewer, 1926, to be a.o.iO" 19 
at 11, 3.4.IO- 19 at i5, 5.3. io- 19 at 19 and I2.2.IO- 19 at a6.5. 

Subsequent determinations by Brodsky, 1929, gave the following values: 
2.22 x io" 19 at 10.8, 3.31 x io~ 19 at 14.9* 5.42 x io" 19 at 19.2 and 
15.1 x io"* 19 at 26.5. 



HYDRARGYRUM CHLORIDE (ic) 

SOLUBILITY OP MERCURIC CHLORIDB IN WATER. 

Average curve from results of Etard, 1894; Foote, 1903; Osaka, 1 
Herz and Paul, 1913; Greenish and Smith, 1903; Schreinemakers and Thonus, 
1912; Sherrill, 1903; Morse, 1902. 
C 1 



t o Gins. HgClj per t o Gms. HgCl 2 per * Gms. HgCl a per 
* * zoo Gms. Sat. SoL 100 Gms. Sat. Sol. * * 100 Gms. Sat. SoL 

o 3.5 25 6.9 80 23.1 
io 4.6 30 7.7 ioo 38 
iS-5 5-3 <&5= 1-047) 40 9.3 120 59 
20 6.1 60 14 150 78.5 

SOLUBILITY OF MERCURIC CHLORIDE IN WATER. 




d of 


Gin*. JftfCls 


d 


of 


Gms. HjfCU 


t- 


sat. sol. 


per 100 


gins, 


. sat, 


. sol. 


f. 


sat 


. sol. 


per ion gms. 


. sat. 


sol. 


18 


_ 


6. 


2-i 


(l) 




56 


1 


TOO 


j3 - 






25 




6. 


^"t 

76 


\ l / 

Ca) 




80 


j 


/ 




n \ 




34 


T.068 


8. 

TUT 1 


/ x/ 

55 


\ A S 

(3) 

i i 


U) 

> 


IOO 


I 


348 


seio 


(3) 













(i) Laird, 1920; (2) Moles and Marquina, 1914, 1924," (3) Tourneux, 1919; 
(4) Toda, 1921. 

More recent determinations have given the following results: 



c o 


d Of 


Oms. HgCl 2 per 


r o 


Qns. HgCl 2 per 


,0 


Oms. HgCl 2 per 




sat. sol. 


100 gps. sac. sol. 


L 


100 0ns. sac. sol. 


c 


100 gms. aat. sol. 


15 


1.0457 


5.426 (l) 


105 


38.9 (5) 


157 


80.0 


20 


1.0518 


6.167 d) 


116 


49-0 


165 


82.6 


25 


1.0560 


6.806 d) 


123 


55-3 


175 


86.5 


25 





6.584 (a) 


129 


61.5 


182 


88.8 


25 





6.732 (3) 


133 


65.1 


195 


91.4 


30 





7.55 U) 


141 


70.6 


206 


93.0 


70 





19.12 (4) 


145 


73-2 


235 


96.0 



(i) Flftttmann, 1928; (2) Benrath, 1927; (3) Benrath and Ammer, 1929; 
(4) Sugrten, 1929; (5) above 100, Benrath, Gjedebo, Schiffers and 
Minderlich, 1937. 



6 2i HYDRARGYRUM 

EQUILIBRIUM IN THE SYSTEM MERCURIC CHLORIDE, MERCURIC IODIDE AND WATER. 

(Sugden, 1939.) 

Suitable mixtures of the two salts in water were heated to 100 and 
then rapidly filtered. The solutions thus obtained, from which solids 
separate, w*re rotated up to 11 days. It was necessary to operate in 
this manner since equilibrium is established too slowly if solids are 
present from the beginning . Due to analytical difficulties great ac- 
curacy is not claimed for the results. The solid phase in the iodide 
region consists of two series of mixed crystals which are respectively 
yellow and red. They correspond to the yellow and red form of the 
simple iodide stable above and below 129. 

Results at 70 



fas. per 100 g 


pin. sat. sol. 


Solid 


On 3. per 100 gms. 


sac. sol. 


Solid 


HgCl ? 


Hgljj ~^ 


Phase 


HgCl 2 


HgI 2 "^ 


Phase 


7.55 


0.0 


V 


19.12 


0.0 


Vf 


7.6? 


O.q.1 


it 


19.5 


0.44 


ii 


7.75 


0.21 


it 


20.5 


1.10 


Y 


7.77 


0.43 


11 + R 


19.8 


1.02 


" 


7.72 


0.54 


R 


17-4 


0.99 


it 


7.69 


0.46 


tt 


16.7 


1 .00 


11 


6.75 


0.31 


it 


12.8 


0.99 


H 


5-32 


0.28 


" 


12.6 


0.94 


ii 


3-39 


0.33 


H 


10.2 


0.91 


" + R 


2.20 


0.18 


" 


9.9 


0.84 


" t R 


7.82 


0.52 


Y 


7-35 


0.75 


R 


5.36 


0.37 


11 


3.94 


0.52 


M 



W = White, R = Red, Y = Yellow. 
MERCUROUS CHLORIDE HgCl 

SOLUBILITY OF MERCUROUS CHLORIDE (CALOMEL) IN AQUEOUS SOLUTIONS OF 
SODIUM CHLORIDE, BARIUM CHLORIDE. CALCIUM CHLORIDE AND OF HYDRO- 
CHLORIC ACID AT 25. (Richards and Archibald, 1902.) 

Solid phase in each case. Calomel + about o. i gm. of mercury. 



In Aqueous NaCl. 



In Aqueous BaCl 2 . 



Sp. Gr. of 


Gms. T>er Liter. 


Sp. Gr. of 


Gms. per Liter. 


Solutions. 


r NaCl. 


HgCl. ' 


Solutions. 


' BaCl 2 . 


HtfU. 




5.35 


0.0041 


1. 088 


104.15 


0.044 


.040 


58.50 


0.041 


I-I34 


156.22 


0.088 


.078 


IIQ 


0.129 


I.I74 


208.30 


O.IO7 


093 


148.25 


0.194 


1.263 


3I 2 -54 


0.231 


.142 


222.3 


0.380 








.188 


292.5 


0.643 










In Aqueous CaClf. 






In Aqueous HC1 




Sp. Gr. of 


Gms. i>er Liter. 


Sp. Gr. of 


Gms. per 


Liter. 


Solutions. 


' CaCl 2 . 


HgCl. * 


Solutions. 


' HC1. 


HgCl. ' 


. . . 


39-96 


O.O22 




31.69 


0.034 


. . . 


55-5 


0.033 




36.46 


0.048 


1.064 


in 


O.oSl 


1.042 


95-43 


0.207 


I.I05 


138.75 


0.118 


1.069 


158-4 


0-399 


I.ISI 


195-36 


0.231 


.091 


209.2 


0.548 


1 .205 


257-52 


0.322 


.114 


267.3 


0.654 


I- 2 43 


324.67 


0.430 


.119 


278.7 


0.675 


L3I5 


432.9 


0.518 


.132 


317.3 


0.670 


1.358 


499-5 


0.510 


153 


364.6 


0.673 



100 gms. bromoform, CHBr 3 , dissolve 0.055 gin. HgCl at i8-20. (Sulc., 1900.) 
Data for the system Mercurous Chloride + KOI! T H g O at 25 are given 
by Herz, 1911. 



Cl 



HYDRARGYRUM 



622 



MERCURIC CHLORIDE HgCl 2 

SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SALT SOLUTIONS AT 25*. 

(Herz and Paul. 1913-) 



In Aqueous Ba- 
rium Chloride. 

Mols. per Liter. 


In Aqueous Cal- 
cium Chloride. 

Mols. per Liter. 


In Aqueous Lith- 
ium Chloride. 

Mols. per Liter. 


In Aqueous Mag- 
nesium Chloride. 

Mols. per Liter. 


BaCl t . HgU,. 

o 0.265 

0.385 0.697 
0.572 1.167 
0.776 1. 6*2O 
1.336 2.645 
3-030 5-348 


~CaCl 2 . HgCl 2 . 
O.IQO 0.364 
O.4O2 0.766 

0.656 1.108 
0.964 1.811 
1.429 2.645 
i.7 2 3 3-304 


LiCl. HgCl 2 . 
0.414 0.351 

0.835 0.666 
1.271 1.021 
1.738 1.678 
2.265 2.214 
3.091 2.896 


JMgCV HgCl 2 . " 

0.168 0.374 

0.415 0.719 
0.570 I.I3I 
0.997 1.864 
I.32O 2.569 
1.728 3.206 



Cl 



In Aqueous Potas- 
sium Chloride. 

Mols. per Liter. 


In Aqueous Sodium 
Chloride. 

Mols. per Liter. 


In Aqueous Strontiu 
Chloride. 

Mols. per Liler. 


' KG. HgCV 

o 0.265 

O.I 0.381 (Sherrill, 1903.) 
0.174 0.355 
0.221 0.381 
0.25 O . 542 (Sherrill, 1903.) 
0.683 0.836 


' Nad. HgCV 
O.2OI 0.372 
0.416 0.508 
0.671 0.748 
I.I53 I.IQ2 
I.94I 2.O22 
3.162 3.434 


SrCl 2 . HgU,. 
0.164 0.315 
0.3II 0.563 
0.519 0.829 
0.724 1.342 
1.046 1.776 
1.384 2.293 



SOLUBILITY OP MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OP 
HYDROCHLORIC ACID AT: 



0. 


20-25 (?). 


(Engel Ann. chim. 


phys. [6] 17. 362. '9.) 


(Ditte/Mtf. [5] 22, 551, 8i.) 


Mg. Mols. per 


zoo cc. Sol. 


Gms. per 


loo cc. Sol. 


Sp. Gr. of 


Parts HC1 


Parts HgCl 2 


HQ. 


*HgCL 


HC1. 


HgCl 3 . 


Solutions. 


per 100 
Parts H 2 O. 


per 100 
Parts Solution 


4-3 


9-7 


i-57 


I 3 .II 


I.II7 


o.o 


6.8 


9-9 


19.8 


3-6i 


18.04 


1.2 3 8 


5-6 


46.8 


17-8 


35-5 


6.49 


32-44 


1.427 


10- 1 


73-7 


26.9 


55-6 


9.81 


49.04 


1.665 


13-8 


87.8 


32-25 


68.9 


11.76 


58.80 


1.811 


21 .1 


127.4 


34-25 


72.4 


12.48 


62 .40 


1.874 


3 I.O 


141.9 


4L5 


35 5 


15 -13 


75^5 


2.023 


50-0 


148.0 


4 8.1 


88 6 


17-54 


87.70 


2.066 


68.0 


154.0 


70.9 


95 7 


25.84 


129.20 


2.198 







One liter of o.inHg(NOj) 2 solution dissolves 105 gms. HgCl 2 at 25. 

.... (.Morse, 1902.) 

This result, together with distribution experiments, show that complexes of 
HgQ, and Hg(NO,), are formed. 



623 



HYDRARGYRUM Hg 



EQUILIBRIUM IN THE SYSTEM MERCURIC CHLORIDE, YELLOW MERCURIC OXIDE 

AND WATER AT 35. (Toda, 1921. j 

The various mixtures were rotated in a thermostat for about 72 hours, and 
both the clear solution and solid phases were analyzed. 



Gms. per 100 gins. sat, sol. 



HgCl,. 


HgO. 


8.58 


0.0 


8.72 


o. 14 


8.68 


0.07 


8.69 


O.IO 


8.81 


o.o3 


8.70 


O.II 


8.69 


0. IO 


4.3 9 


0.09 


3.42 


0.06 


0.66 


0.02 


0.66 


O.O2 



Solid Phase. 

HgCl 2 

>H-HgCl 9 .2HgO 



HgCI,.aHgO 




Solid Phase. 

HgCMHgO 



HgO 



EQUILIBRIUM IN THE SYSTEM MERCURIC CHLORIDE, POTASSIUM CHLORIDE, 

AND WATER AT 34. ( Tourneux, 1919. ) 

Saturation was secured by constant stirring. Both the saturated solutions and 
solid phases were analyzed. 

Gins. C 1 

per 100 gms. 

s;vl. sol. 
d of 
id. sol. 

.386 
.368 
.4^8 
.56i 
.620 
.624 
.621 



.459 



Results similar to the above are given for 56, 80 and 100. 

In a later paper by Tourneaux, 1934* having for its object an expla- 
nation of the variation in the solubility of HgCl- in aq.. solutions of 
KC1 and vice versa, the author calculates the equilibrium constants 
involved and .finds that they vary with the temperature in accordance 
with the law of Van't Hoff. 

Data for the system HgCl 2 + KCI -f NH^Cl + H 2 at 25 are given by Osaka 
and Ando IQ25, 1926. 







Gm 


s. 






per 100 


gms. 






sat. * 


ol. 




d of 


* ^ * 


*~**~^ 


s 


at. sol. 


HgCl s . 


KCI. Solid Phase. 


I 


.068 


8.55 


HgCl 2 


I 


.202 


19. 14 


2.6 




- 


27.2 


4.2 




- 


34.1 


5.4 


I 


497 


37.0 


6.0 


I 


.512 


37.4 


6.O -H2HgClj.KC1.2lf s O 


1 


.520 


3 7 .8 


6-5 2iigCi 2 .KCi.2ir a o 


I 


,533 


37.7 


6.7 


I 


.545 


37.6 


7-3 ^ WCI , K1 . no 


I 


.549 


3 7 .8 




I 


.534 


37.4 


7.8 3HgCl s .2KCl./ 3 HsO 


I 


.53o 


3 7 .6 


8.0 


I 


.524 


36.8 


8.2 -f-IIgCl 9 .KCl./*HiO 


I 


.512 


35. q 


8.2 HgCl 9 .KCl.V<H*0 


I 


.486 


34.5 


8.5 



Hg C1 2 . 


K Cl. Solid Phase. 


'^7-9 


9.6 HgCl s .KCl./ 4 H s O 


25.5 


11.4 


26.8 


i 4 . 9 


3o.8 


20.0 


32.6 


22 . 


33.o 


21-9 +IfgCl,.2KCUH a O 


32.8 


2t.9 HgCl 9 .SKCl.H 9 


29.0 


23.0 


24.5 


24-8 


20. 65 


26.0 4-KCl 


7.8 


26 .8 KCI 


12.2 


27.0 


8.4 


2 7 .3 


4.5 


27 . 5 


0.0 


27 . 8 



Hg HYDRARGYRUM 62 4 

SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM 
CHLORIDE AT 20 AND VICE VERSA. 

(Tichomirow, 1907: see also results by Foote and Levy 



Gms. per 100 Cms. HO. 



Cms. per 100 Gms.1^0. 



KG. 
O 


HgCU. 

7-39 


solid rnasc. 

HgCfe 


r KC1. 

20/35 


HgCl.,. 

29 HgCi 2 .KCl 


1. 12 


11.63 


(I 


26.31 


34.83 " 




2-39 

4. os 


I5-72 
22.17 


It 

it 


30-32 
34-12 


39.10 
42.82 


" +HgCl 2 .2KCl 


nr J 

4^4 


25.16 


" +2HgCl 2 .KCl 


34.18 


39-34 


HgCl 2 .2KCl 


5.60 


25- X 3 


2 HgCl 2 .KCl 


34-34 


35-i 6 


" 


6. 7 I 


25.66 


". 


35-54 


30.63 


a 


7-39 


26.41 


" +HgCl 2 .KCl 


37-72 


24.30 


it 


7.46 


24.70 


HgCl 2 .KCl 


41-33 


19-33 


" +KC1 


8-95 


x 9-93 


a 


39-66 


I5-76 


KC1 


t5 


22.87 


n 


37.87 


10.28 


" 


t?-S7 


26.12 


tt 


35-32 


21 


it 



Cl 



SOLUBILITY OF MIXTURES OF POTASSIUM AND MERCURIC CHLORIDES 
IN WATER AT 25. 

(Foote and Levy.) 



Composition of Solution. 
Grams p~r too Grams 
Solution. 


Percentage Composition 
of Undissolved 
Residue 


Solid 
Phase. 




KG. 
26.46 
26.24 
26.43 
26-33 


HgC! 2 . ' 

none 
15.04 
15.02 
15.02 


KC1. 
100 


HgClo. 

none 

3-63 
26.15 
52.01 


H 2 0. 


KC1 

KC1 and 
2KCLHgCl 3 .H 2 O 




26.33 


14.92 




61 .04 








23-74 


18.91 


34.61 


61.66 


3-73' 


2KCl.HgCl 2 .H 2 O 




22.36 

21.39 


21-39 
23.88 


34-77 
34.80 


62.02 
61.84 


3-21 
3-35; 


K Calc. Composition 
34-05% KC1.6t.8 4 %HgCl* 


20.32 


27.62 




65.24 




2KCl.HgG 2 .H 2 O and 




20.26 


27.38 




73-98 




KCl.HgCl 2 .H 2 O 




17-85 


25-34 


21.89 


75-io 


3.01^ 






9.26 
7.80 
6.84 


18.95 
19.56 
22.81 


21 .02 
20.76 
20.75 


73-36 
73.06 

74-54 


5-62 
6.18 
4.71 


KCl.HgCl 2 .H 2 

Calc. Composition 
ao.52%KCU 74-53% HgCl 2 , 
4-95% H 2 


6.66 


24.32 


20.54 


73-99 


5-47. 






6.52 


25^3 




76.46 




1K.Cl'HgC] 2 .H 2 O and 




6.64 


25.16 




80.60 




K C-l .2 HgCl 2 <2 H 2 O 




6.27 
5*77 


25.11 
24.73 


12.09 
11.87 


83.20 
83-18 


4-71 
4.95 


|KC1.2HgCl 2 .2H 2 O 
Calc. Composition 




4.68 


24.75 




84.46 








4.66 


2 5- I 7 




93.68 




I KC1.2HgCl 2 .2H 3 O and 


HgClj 


4.69 


24.82 




98.50 




j 




none 


6.90 


none 


100. OO 


none 


HgCl, 





62 S 



HYDRARGYRUM Hg 



Data for the quaternary system Ammonium Chloride +' Mercuric Chloride 
Potassium Chloride + Water at i5 arc given by Osaka and Ando, 192^. 



The results of these authors have been further interpreted in a 
paper by Janecke, 1938. 

Data for equilibrium in the system H?C1 8 KOI1 + H g O at 25 are 
given by Herz, 1910. 



SOLUBILITY OP MERCURIC CHLORIDE IN AQUKOUS SOLUTIONS OF 
MAGNESIUM CHLORIDE AT 25 AND \fiCE VERSA. 

(Bassett, Barton, Foster and Patenan, 1933.) 



QMS. per 100 
gns. sat, sol. 



Solid 
Phase 



6.90 
33-47 
47.72 
56.03 
57.46 
59-23 
55.90 
55.78 
54.53 



0.0 

5.4 
8.28 

9.86 
10.68 
12.48 
14.44* 
14.38 
15.24 



Ctas. per 100 
gms. sat. sol. 


53^15 


16.30 


51.88 


17.27 


50.08 


18.77 


49.85 


19.23' 


49-47 


19.07 


48.95 


19.22 


48.78 


19.45 


47-32 


20.01 


45-45 


20.90 



Solid 



Ons. per 100 
gms. sat. sol. 


Solid 
Phase 

C 

M T 

D 
it 

II 

II 


44.93 
43-20 
41 .66 
31.92 
24.29 
11.76 
0.58 
0.0 


21.12 
21.95 
22.43 
25.29 
27.64 
31.72 
35.48 
35-70 



* Metastable 
B = [M?(H 8 0) fl ] 



; C = 



[H?C1 4 ] ; D - 



Cl 



SOLUBILITY OP MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OF 

SODIUM CHLORIDE. 

(Homeyer and Ritsert Pharm. Ztg-33, 738, '88.) 

Per cent Concentration Gms ' HgC1 * *** 10 Gms ' NaC1 &***< at: 

of NaCl Solutions. 

o-5 
i.o 



10. 

25-0 



26.0 (saturated) 128 



j o 


65 


100 


10 


13 


44 


14 


18 


48 


30 


3* 


64 


58 


68 


no 


I2O 


142 


196 


128 


152 


208 



100 ?ros. of aqueous i.o normal NaCl solution dissolve 25.08 pms. 
at 25. (Osaka, 1903-08.) 



Hg HYDRARGYRUM 



626 



EQUILIBRIUM IN THE SYSTEM AMMONIUM CHLORIDE, MERCURIC CHLORIDE, 

WATER AT 30. 

(Meerburg, 1908.) 



jms. per too Gins. Sat. Sol. goijd 


HgCl 2 . 


NHiCl. Pa**- 


O 


29 . 50 NH.C1 


22.8O 


26.91. " 


42.45 


25.05 


50.05 


24.79 " I ' 2 ' 1 


53-08 


22-77 1.2.1 


58.90 


20.02 " +1.1.1 


56.38 


18.50 i-i.i 


55.58 


16.82 


57-01 


14.12 " +3.2.1 


56.26 


13.04 3.2.1 



Gms. per roo G 


ms. Sat. Sol. 


Solid 


' HgCl 2 . 


NH 4 C1/ 


Phase. 


57.05 


9.92 


3-2.1 


58.65 


9.20 


" +9-2 


ISl-83 


8.76 


9.3 


*46 


7.52 


" 


*3S-6o 


5.26 


" 


*32.9o 


5-06 


' 


29.65 


3.62 


" +HgCl, 


40.12 


5-13 


HgCl, 


21 


2.29 


" 


7.67 


O 


" 



1.2.1 = HgCi 2 .2NH4Ci.H 2 O; i.i.i = HgCkNHi. 
3.2.1 = 3HgCl2.2NH4Cl.H,0; 9.2 = 9 HgCl 2 .2NH 4 Cl. 

1 In these solutions 2 to 3 weeks were required for attainment of equilibrium. 



Cl 



SOLUBILITY OF MIXTURES OF SODIUM AND MERCURIC CHLORIDE IN 

WATER AT 25. 

(Foote and Levy Am. Ch. J. 35, 339, '06.) 

Solid 



NaCl. 
26.5 

18.66 

18.71 
18.64 
18.87 


HgCl 2 . 

none 

51-35 
51-32 
51.42 
51 .26 


NaCl. 
100 


HgCl 2 . 

none 
16.39 
21.98 
65.42 
71.25 


H 2 O. 

none 


fnase, 
NaCl 

NaCl and 
' NaCl.HgCl a .aHaO 




14.97 


57-74 


16.38 


74.18 


9.44' 


Double Salt 




14.03 
13.25 


59.69 
62.16 


16.36 

16.16 


74.21 
74.70 


9-43 
9.14 


NaQ.HgCl 2 . 2 H 2 O 
Calc. Comp. = t6.oT% 
74.14% HgCl.g.85% 


NaCl 
H 2 


13 .17 


62.59 


15.96 


74.76 


9.28 , 






12.97 


62 .50 




78 . 20 








13.14 


62.48 




88.64 




" andHgClj 2 






62-55 




90.83 








Two determinations made 


at 10.3 gave: 








19.46 


46.49 


67.46 


29-19 


3.35 




19.48 


46-50 


22.83 


68.85 


8.32 





627 



HYDRARGYRUM Hg 



SOLUBILITY OF MIXTURES OF MERCURIC AND RUBIDIUM CHLORIDES IN 
WATER AT 25. 

(Foote and Levy, 1906.) 



Composition of Solution. 
Cms. per 100 Cms. Solution. 



Percentage Composition of 
Undissolvecl Residue. 



Solid Phase. 



RbCl. 


HgCl, 


RbCl. 


HgCl 2 . 


H 2 0. 


48.57 


none 


100 


none 


none RbCl 


46.76 


9.18 


88.04 


11.24 


0.72 




47-54 
47-55 


9-49 
9-39 


60.33 
56.59 


37.51 
40-75 


2.16 
2.66 


RbCl and 2RbCl.HgCl 2 .H 2 


47-3 
47-65 


9-47 
10.35 
19.58 


46.73 
46.50 


49-38 
50.92 
50.80 


3-88 
2.58 
3.22 


2 RbCr.HgCI 2 .H,0 Calc. Com- 
position 45-55% RbCl. 51 -05% 
HgCl 2 . 3 -4%H 2 


34-77 


19.94 


43-07 


52.44 


4-49 


2RbCl.HgCl 2 .H 2 and 3RbCl. 


34'76 


20. 10 


41 .IO 


55 -36 


3-54. 


2 HgCl 2 .2H 2 O 


30.27 


20.17 


39-07 


57-34 


3-59 


3 RbC1.2HgCl 2 .2H 2 
Calc. Composition 


29.20 


20.55 


39.10 


57-47 


3-43 


38.55% RbCl, 57-62% Hga 2 . 


27.38 


20.63 


38.67 


57-40 


3-93 


3.82 %H 2 


26.83 


20.87 


38.48 


57.36 


4.16 


3 RbC1.2HgCl 2 .2H 2 O and 


27.09 


20.97 


31.40 


64.35 


4.25 


RbCl.HgCl 2 .H 2 


26.15 


20.58 


30-34 


65.48 


4.18 


RbCl.HgCl 2 .H 2 


23-81 


18.71 


30.87 


65.10 


4-03 


Calc. Composition 


18,10 


14-25 


29-87 


65.28 


4 85 


29.49% RbCl, 66.11% HgCU, 


10.87 


10.42 


29-33 


66.15 




4.40% H 2 O 


10.68 


10.56 


28.59 


67 99 


3-42 


RbCl.HgCl 2 .H 2 and 3 RbCl 


10.50 


10.05 


26.22 


72.20 


1-58 


4 HgCl 2 .H 2 


10. 06 


9.86 


25.28 


73 -38 


0.84' 




8.48 
8.46 


8.71 
8.80 


25-30 
25-44 


73 15 
73-67 


0.89 


3RbC1.4HgCl 2 .H 2 O 
Calc. Composition 
24.76% RbCl, 74.01% HgClj, 


5 68 


8.70 


25.09 


73-46 


1-45 


i.2 3 %H 2 


5 - IO 


8-33 


24.92 


73-93 


1.15 




3 43 


8.25 


22.79 


75-72 


1 .49 


3RbCl. 4 HgCl 2 .H 2 and 'RbCl 


3-38 


8 


12.68 


86.74 


0.58 


5HgCl a 


2.98 
1.89 


7.71 
7.64 


8.40 
8.38 


91.24 
91.78 




RbC1.5HgCl 2 
Calc. Composition 


1.50 


7-55 


8.30 


91 81 




8.20% RbCl, 91.8% HgCl, 


1. 10 


7 21 


8.07 


91.58 






o 79 


7.16 


6 91 


93-15 




RbCl.sHgCl 2 and HgClj 


0.84 


7-42 


2 .27 


97-09 






none 


6.90 


none 


100 


. . . HgCl 2 



Cl 



Hg HYDRARGYRUM 

MERCURIC CHLORIDE HgCl ? 



Cl 



628 



SOLUBILITY OK MERCURIC CHLORIDP, IN AQUEOUS SOLUTIONS OP 
STRONTIUM CHLORIDE AT 25 AND VICE VERSA. 

(Bassett, Barton, Foster and Pateman, 1933.) 



Ons. per 100 

0ns. sat. sol. Solld 
,5. ^...__ x Phase 


Otos. per 100 Gfcns. per 100 
gjns. sat. sol. Solld 8*8. sat, sol. ^ 


Solld 
Phase 


'HgCl ? SrCl^ *** HgCl 2 SrCl 2 


6. 


90 





.0 HgCl, 


56. 


20 


19.20 B - 


S o. 





40 


.0* 


D 


34. 


70 


9 


30 " 


55- 


45 


19.82 


48. 


20 


23 


.60 


E 


48. 


21 


13 


93 " 


54. 


33 


20.88 


46. 


25 


24 


.02 




56. 


62 


16 


.65 " 


52. 


70 


21.90 


45* 


32 


24 


.26 




57. 


17 


17 


34 " 


51- 


20 


22.50 


34- 


52 


26 


.78 




58. 


38 


18 


.02 " +B + S 


50. 


87 


22.98 


31- 


02 


27 


50 




58. 


68 


18 


.47* " + C 


118. 


90 


23.69 


+ E 18. 


82 


30 


.50 


" 


58. 


<J9 


19 


.42* C 


48. 


8l 


24.01 


8. 


55 


33 


.42 




59. 


49 


19 


.66* " 


48. 


77 


23.90* " o. 





35 


.84 




58. 


13 


18 


.00 B + S 



















= Me last able 



SrCl 



B = [Sr(lLO) R j [(HgClJ.Cl 
CU.2ILO; E 5 SrCl p .6H 2 0; ! 



J; C = [Sr(H 2 0) 6 ] [<HgCl ? ) 6 Cl 2 ] ; D = 
> r solid solution. 



SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS ETHYL ALCOHOL AT 25 

(Abe, 1912.) 



C,HOH. HgCl,. 


oouarnuc. - ^^ 


HgCl 2 . ' -" u - ase - 


o 6.80 


HgCk 45 84 


15-36 


HgCl 2 


5.08 6.65 


" 49.86 


18.18 


u 


14.49 6.41 


536i 


21 .40 


a 


21 6.55 


57.26 


24.51 


" 


26.25 7.31 


;; 60.55 


27.67 


<< 


31-53 8.51 




29.86 


(C 


36.85 10.32 


" 67.39 


32.40 


<( 


41.36 12.64 


(C 






SOLUBILITY OF MERCURIC CHLORIDE IN AQ. ETHYL ALCOHOL 


AT 25. 




(Herz and Anders, 1907.) 






Wt. % C 2 H 6 OH 
in Solvent. 


d^ of Solvent. d^ of Sat. Sol. 


Cms. HgCV 
100 cc. Sat. ! 


per 
Sol. 





0.9971 1-0565 


7.22 




20. l8 


0.9665 I.O2I4 


6.76 




40.69 


0.9302 I.OlSo 


10.69 




70.01 


0.8632 I. O6l6 


23.60 




100 


0.7856 I.I067 


36.86 





The solid phase in contact with solutions of Mercuric Chloride plus 
Potassium Chloride in 95* or absolute ethyl alcohol at 34 was found to 
be 6II?Cl ? .5KCl.aC g H 6 OH. (Pernot, 1934.) 



629 HYDRARGYRUM 

SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS METHYL ALCOHOL AT 25*. 

(Herz and Anders, 1907.) 



Wt. % CH 3 OH 
in Solvent. 


dy. of Solvent. 


(/ of Sat. Sol. 


Gms. HgCl 2 
100 cc. Sat. ! 


10. 60 


0.9792 


1.0441 


7.90 


30-77 


0.9481 


I.O42O 


11-31 


37.21 


0.9369 


1.0507 


13-43 


47-06 


0.9186 


1.0809 


19.71 


64 


0.8800 


I.20I5 


38.44 


78.05 


0.8489 


1.3314 


57-17 


IOO 


0.7879 


I. 2l6o 


48.62 



loo cc. 90% ethyl alcohol dissolve 27.5 gms. HgCl 2 at 15.5, d i& sat. sol. = 1.065. 

(Greenish and Smith, 1903 J 

loo gms. 99.2 % ethyl alcohol dissolve 33.4 gms. HgCU at 25. (Osaka, 1903-8.) 

abs. " " " 49.5 " " " . (de Bruyn, i8 9 a.) 

" methyl " " 52.9 " " at 19.5 and 66.9 gms. at 25. 

(de Bruyn, 1892.) 
" " 1.2 " " at the crit. temp. 

(Centnerszwer, 1910.) 

SOLUBILITY OP MERCURIC CHLORIDE IN METHYL, ETHYL PROPYL, 
n BUTYL, Iso BUTYL AND ALLYL ALCOHOLS. 

(Etard Ann. chira. phys. [7] 2, 563, '94.) 

NOTE. For the solubility in Me, Et, and propyl alcohols at room C 1 
temperature, see Rohland Z. anorg. Ch. 18, 328, '98; at 8.5, 20 and 
38.2, see Timofejew Compt. rend. 112, 1224, '91; in Me and Et 
alcohols at 25, see de Bruyn Z. physik. Ch. 10, 783, '92. The deter- 
minations of these investigators agree well with those of Etard, which 
are given below. 

Grams HgClg per 100 Grams Saturated Solution in: 



b . 

""""* ^?O 


CH 3 OH. 


14-5 


C&EfyOH. CHg(CH2)30H. (CHg^CHCHsOH. 

i s .o 


CH 2 .CH,CH,OH 


20 


. . . 


20.1 


*5 -7 


*3 *5 




21 .0 


10 


15-2 


26.5 


16.5 


13-7 




25-5 


o 


2O. I 


29.8 


17.4 


14.0 


5** 


30.0 


+ 10 


26.3 


30.6 


18.0 


14-3 


6.0 


37-5 


20 


34-o 


32.0 


18.8 


i 4 .6 


6.8 


46.5 


25 


40.0 


32-5 


19-5 


'S-S 


7-2 




30 


44-4 


33-7 


-2O.O 


16.5 


7-S 




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 - 


24.9 




IOO 


70.1 


54-3 


43-8 




31 .7 




120 


73-5 


61.5 


50.6 




39-2 




ISO 


78-5 








... 


... 



SOLUBILITY OF MERCURIC CHLORIDE IN AQ. ETHYL ACETATE AT 25. 

(Herz and Anders, 1907.) 

wt * 



V f Solvent - V f Sat - SoL 

o 0-997 1 1-0565 7.22 

4.39* ... 1.0581 7.38 

96.76! - 1-2371 41.55 

100} 0.884 1.1126 26.42 

Almost sat. with ethyl acetate. | Ethyl acetate almost sat. with H^O. J (b. pt. - 75-77.) 



HgHYDRARGYRUM 630 



SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS 

OF ETHYL ALCOHOL AT 18. 

(Laird, 1920.) 

AVt. % <' 4 H,OH <ims. HgCl, Wl. %> C 8 H.,OH Gms. HgCl s 

Insolvent. p<.*r iuo gins. sal. sol. in solvent. per too #ms. sat. sol. 

o 6.24 a5.o 5.o8 

10. o 5.63 3o.o 5.86 

i5.o 5.43 4o.o 7.58 

20 . o 5 i 5 5 i . o i i . 3o 

SOLUBILITY OF MERCURIC CHLORIDE AT 23 IN AQUEOUS SOLUTIONS OF 
( Moles and Marquina, 1914, 1924. ) 

Citric Add. Tartarlc Acid. Glyeerol. Sucrose. 



Percent Gins HgClj Percent Gins. II# CI 3 Percent Gins fig (U. Percent Gms. HgClj 

Citric acid per lOOjsms. Tartarlc acid pcrioogius. Glyeerol per lOOgms. Sucrose per 100 gms. 
Insolvent. sat. sol. Insolvent. sat. sol. insolvent. sat. sol. insolvent. sat. sol. 

o.o 6.76 10. o 6.36 5.o8 7.20 io. o 7.08 

jo.o 6.63 20.0 5.75 i5.i 8.33 25. o 8.o5 

25.o 5.73 '25.o 5.36 25.o 9.60 3o.o 8.46 

5o.o 3.99 35.o 4.59 35.o 1 1 . io 35. o 8.83 

42.5 3.98 5o.i8 14.88 4o.o 9.14 

5o.o 3.28 75.08 26.53 42.5 9.16 

00.00 44-22 47-0 9.68 

55. o i o.i 4 

Ethyl ether, saturated with mercuric chloride by repeated agitation at room 
temperature, and also by prolonged boiling under a reflux condenser and allowing 
to stand at ordinary temperature for many days, contained 6.9 gms. Hg C1 2 per 
100 gms. ether. On the basis of 0.720 as the Sp. Gr. of the ether this corresponds 
to 5.o gms. Hg C1 2 per 100 cc. of ether. ( Richard, 1926.) 

100 gms. glycerol of d = 1.23-26 (= 86.5 o/) dissolve 53.5 gm. HgClj at 20 
d= 1.2645 (= 98.5 o/ ) 65.5 

(Holm, 1921, 1922.) 

100 gms. sat. solution of mercuric chloride in selenium oxychloride (Se C1 2 ) 
contain 0.89 gm. Hg C1 2 at 25. ( wise, 1923. j 

100 gms. liquid Sulfur Dioxide dissolve 0.103 8 m ' HgCl 2 at o. 
(Jander and Ruppolt, 1937.) 

SOLUBILITY OP MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OF URETHAN AT 25. 

(Falltzsch, 1928, 1929.) 

On. Mols. HgClgjper 1000 grca. i^p Solid 

_.^ ^ NHgCOOCgHg "^ Phase 

0.2? 0.0 H S C1 - 2 
0.30 1.1225 " 

0.607 4.4898 " 

1.552 11.326 " 

0.25 51.79 " ^ NH E COOC 2 H 5 



631 HYDRARGYRUM 

SOLUBILITY op MERCURIC CHLORIDE IK ANHYDROUS ACETIC ACID 
DETERMINED BY THE SYNTHETIC METHOD. 

(Davidson and Chappell, 19W-) 






MOlS. 1 




per Solid 


..0 


Mols. Hi 


jClp per 


Solid 


C 


100 fflOls. Hj 


2, ** 


CHgCOOH Phase 


c 


100 mols. H(jCl ? + CH^COOH 


Phase 


16.6 





.0 


CH,COOH 


'53 


1 


.46 


IlgCl. 


16.45 





.27 


M 


Co 


1 


.6l 


it ' 


16.35 





.477 


" 


66 


1 


.8l 


it 


17-0 





477 


HgCl 2 .2CH 3 COOH 


72 


2 


.01 


11 


24 





.680 


11 


78 


2 


.22 


it 


30 





936 





84 


2 


.42 


it 


33 


1 


.06 


11 


92 


2 


.74 


M 


36 


1 


.19 


11 


97 


3 


.05 


M 


40 


1 


-15 


HgCL 8 


106 


3 


55 


" 


46 


1 


30 


" 


117 


^ 


.2.1 





DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND BENZENE. 

(Linhart, 1915.) 

Results at 25. Results at 40. 

Mols. HgCU per Liter: Cone, in H 2 O Mols. HgCl* per Liter: Cone, in H a O 

CH 8 Layer. H 2 Layer. Cone, in C 6 H 8 CH Layer. H 2 O Layer. Cone. inC 6 H 8 

0.02100 0.2866 13-65 0.02647 0.34600 I3-07 

0.01224 - r 5777 12.91 0.015296 0.18470 12.08 

0.005244 0.064756 12.35 0.011774 0.138228 11.74 

0.000618 0.007382 H-95 0.008041 0.091959 H-44 

0.000310 0.003696 11.90 0.004140 0.04586 11.08 

0.000155 0.001845 11.90 0.000847 0.009153 10.81 



DISTRIBUTION OP MERCURIC CHLORIDE BETWEEN WATER AND AMYL ALCOHOL. 

(Mossnessenstcy and Astachow, 1927.) 

Mola. HgClg^per liter Cone. In H p O 

' Water Amyl Alcohol v Cone. In Anyi Alcohol 

0.0072 0.013 0.554 

0.0378 0.072 0.525 

0.0688 0.139 0.495 



SOLUBILITY OF MERCURIC CHLORIDE IN ACETIC ACID. 

(Etard, 1894.) 



Gms. HtfCl. 
t. per 100 Gms. 


Gms. H K C1 2 
t. per too Gms. t. 


Gms. HgCU 
per loo Gms. 




Solution. 




Solution* 




Solution. 


2O 


2.5 


70 


8.S 


no 


13-6 


30 


3-5 


80 


9-7 


120 


16.5 


40 


4-7 


90 


ii 


130 


2O-7 


50 


6 


IOO 


12.4 


140 


25.2 


60 


7.2 






160 


34.8 



Hg HYDRARGYRUM 632 



DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND ETHER. 

(Hantzscli and Sebalt, 1899.) 

50 cc. ether + 50 cc. sat. aqueous HgCk solution were shaken together at 
different temperatures and after equilibrium was established the HgCla in each 
layer determined. 

Mols. HgCl 2 per Liter: ,/ 



b . 


H 2 Layer (c'). 


(C 2 H fi ) 2 Layer (c 2 ). 


c 2 





0.0056 


0.01407 


0.391 


10 


O.O066 


O.OI4I5 


0.467 


17.5 


O.OOQO 


O.O2I5O 


0.419 


25 


0.0095 


O.O2O76 


0.429 



Determinations by Skinner (1892) at room temp, using concentrations of 
in the aqueous layer varying from 1.4 to 5.9 per cent, gave a distribu- 



tion coefficient, = approximately 0.23. 

Ct 

DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN AQUEOUS HC1 AND ETHER 

AT 18. (Mylius, 1911.) 

When i gm. of Hg as HgCU is dissolved in too cc. of H^O or aqueous HC1 and 
shaken with 100 cc. of ether, the percentage of the Hg which goes into the ethe- 
real layer is as follows: 

Percentage Cone, of Aq. HC1 o (=H20) i 10 20 

Per cent Hg in Ether Layer 69.4 13 0.4 0.2 

DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND TOLUENE AT 24. 

(Brown, 1898.) 
Cms. HgQa per 100 cc. Gms. HgCU per TOO cc. 

' HaO ' CftHgCHs fi& QH^Ctea 

Layer. Layer. Layer. Layer. 

0.442 0.0270 1.816 0.130 

0.732 . 0.0488 3-766 0.292 

0.780 0.0542 3.754 0-298 

1.192 0.0812 6.688* 0.528* 

* This solution saturated. 
Results at Dif. Temperatures. Results at 25. 

(H^nusch and Vagt, ,90!.) ^^4V$"T 

Mols. H&C^pcr Liter: Cj Mols. HgCl 2 per Liter: Cl 



H 2 O Layer (ri). 


C 8 H 5 CH 3 Layer (<. 


c 


H 2 Layer fo). 


C 6 H 8 CH 3 Layer fo). 


<Tj 







O 


.0578 


O 


.0047 


12.35 


O 


.18410 


0.01590 


II 


.6 


IO 





-0575 


O 


.0050 


II. 


60 


O 


.09193 


0.00807 


II 


4 


2O 





.0576 


O 


.OO5O 


II . 


40 


O 


-04593 


O.OO4IO 


II 


.1 


30 


o 


0574 





.0051 


II . 


2O 


o 


.02289 


O.OO2II 


10.8 


50 


o 


0573 


O 


.0052 


II. 


25 


o 


.01142 


O.OOIO8 


10 


5 


0.00573 


O.OOO57 


IO 





Data for the effect of Hg(N0 3 )2 upon the distribution are given by Morse 
(1902). Results for the effect of ZnCk are given by Drucker (1912). 



633 HYDRARGYRUM 

SOLUBILITY OF MERCURIC CHLORIDE IN WATER-ETHER MIXTURES AT 25. 

(Abe, 1912.) 
Cms. per 100 Cms. Sat. Sol. 

Solid Phase. 

HgCl, 

U 



HgCl 2 . 


Ether. 


H 2 0. 


6.92 


87.86 


5.22* 


5-2 


1.2 


93-6 


4.3 


5-2 


90-5 


2.8 


5.4 


91.8 



1.5 5.4 93.1 

* (Solvent, ether sat. with H 2 0.) 

SOLUBILITY or MERCURIC CHLORIDE IN MIXTURES OF ETHER AND ETHYL 



ALCOHOL AT 25 

(Jim. per TOO Gms. Sat. Sol. 



HgCl 2 . 
32.43 
35-50 
37-39 
37.96 
38.24 
37-75 



QH B OH. 
67-57 

58.59 
51 .02 

44.79 
38.69 
32.84 



(Abe, 1912.) 
Gms. per TOO Gms. Sat. Sol. 

rigci,. 

36.29 
34.08 

28.55 
20.67 

5-49 



27.16 
22.48 
I5.2O 

8.97 
O 



SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF ALCOHOLS AT 25. 

(Herz and Kuhn, 1908.) 



In Mixtures of Ethyl and 
Methyl Alcohols. 
%CH 3 OH d of Gms.HgCl 


In Mixtures of Ethyl and In Mixtures of Methyl and 
Propyl Alcohols. Propyl Alcohols. 
2 %C 3 H 7 OH & O f Gms. HgCl 2 % C 3 H 7 OH dmn of Gms. HgCl, 


in 
Solvent. 


Sat. Sol. 


per loo cc 
Sat. Sol. 


in 
Solvent. 


Sat. Sol. 


per loo cc. 
Sat. Sol. 


in TT 
Solvent. Sat. Sol. 


per zoo cc, 
Sat. Sol. 


O 


I 


.107 


36.86 


O 


I 


1070 


36.86 


O 




.2160 


48.62 


4.37 


I 


.130 


39.43 


8.1 


I 


0988 


36.67 


II 


ii 


.2278 


50-34 


10.40 


I 


157 


42.6l 


17.85 


I 


0857 


34.06 


23 


80 


.2848 


57-14 


41.02 


I 


.294 


58.37 


56.6 


I 


0272 


27.11 


65 


20 


-1568 


42.28 


80.69 


I 


.321 


61.67 


88.6 


O 


9854 


21.66 


91 


80 


.0090 


25.09 


84.77 


I 


.288 


57.82 


91.2 


O 


9824 


21.60 


93 


75 


.0029 


23.23 


91.25 


I 


.254 


53.85 


95-2 


O 


9772 


20.87 


96 


6 0.9851 


21.52 


IOO 


I 


.216 


48.62 


IOO 


O 


9720 


20.03 


IOO 


0.9720 


20.03 



SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF ETHYL ALCOHOL AND BEN- 
ZENE AND OF ETHYL ALCOHOL AND CHLOROFORM AT DIFFERENT TEMPERATURES. 

(Dukelski, 1907.) 



In a Mixture of 
one mol. C 2 H50H 
-f one mol. CeH fl . 

Gms. HgClj 
t. per loo Gms. 


In a Mixture of In a Mixture of In a Mixture of 
two mols. C 2 H 5 OH one mol. CiH 8 OH two mols. C 2 H 6 OH 
+ one mol. C 6 H 6 . + one mol. CH 3 C1. + one mol. CHCU. 
Gms. HgCl 2 Gms. H/?CI 2 *Gms. HuClj 
t. per loo Gms. t e . per 100 Gms. t. ncr 100 Gms. 




Sat. Sol. 




Sat. Sol. 




Sat. Sol. 




Sat. Sol. 


-2.5 


15.20 


5.2 


19.45 


-20.5 


3.82 


-20.5 


6.60 


O 


15.40 


O 


20.13 


12 


4-43 





7.69 


6 


16.38 


9.1 


21.65 


O 


4.89 


8 


8.96 


20.5 


18.40 


2O-9 


23.57 


8 


5.37 


23 


10.66 


20.65 


18.50 


24.4 


24.19 


23 


7.12 


38.5 


12.50 


24.5 


19.33 


36.5 


26.53 


38.5 


8.51 


44.2 


14.40 


34.5 


21-34 


53-7 


31.27 


44.2 


9-51 






54-4 


24.84 


74 


38.74 


45.6 


9.98 






54.5 


24.42 















Some of the determinations were made by the direct method of saturating the 
solution at a given temperature and determining the dissolved material by evap- 
orating and weighing. Others were made by the synthetic method of Alexejew. 



Cl 



Hg HYDRARGYRUM 



Cl 



634 



SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF METHYL ALCOHOL AND 
CHLOROFORM, METHYL ALCOHOL AND CARBON, TETRACHLORIDE, AND METHYL 
ALCOHOL AND DICHLORETHANE AT DIFFERENT TEMPERATURES. 

(Dukelski, 1907.) 



In a 


Mixture of 


In a Mixture of 


In a Mixture of 


In a 


Mixture of 


one mol. CH 3 OH 


two mols. CH 3 OH 


two mols. CH 3 OH 


two mols. CH 3 OH 


-f- one mol 


. CHCla. 


+ one mol. CHCU. 


+ one 


mol. CC1 4 . 


-j- one mol. C2H4C12. 







ms. 


H K C1 2 






Cms. HgCl 2 




Gms. HgCl 2 






Gms. HgCl 2 


t. 


pe 


:r IQ 


o Cms. 


t. 




per too Gms. 


t. 


per 100 Gms. 


t. 




per i<5oGms., 






Sat 


. Sol. 






Sat. Sol. 




Sat. Sol. 






Sat. Sol. 


12 




I 


73 


12 




3-33 


O 


5.20 


o 




13-33 


O 




3 


51 







6-73 


7.7 


6.69 


12. 


o 


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 


o 


34.78 


24. 


9 


10 


7* 


24 


-9 


18.45 


35-5 


20.50 


3 


.2 


36.87 


3- 


6 


ii 


.40 


30 


.6 


19.70 


36.1 


21. 80 


37-4 


37-95 


38- 


5 


12 


.02 


38 


5 


20.83 


48.5 


21.90 


45 


9 


39-36 



SOLUBILITY OF MERCURIC CHLORIDE IN MIXTURES OF METHYL ALCOHOL 
AND BENZENE AT DIFFERENT TEMPERATURES. 

(Timofeiew, 1894.) 



In a Mixture of one mol. 

CHaOH 4- one mol. C 6 H 6 . 
+o Gms. HgClj per 100 

1 Gms. Sat. Sol. 



21-25 
30 
37 



8 

23.9 
27.3 
28.1 



In a Mixture of one mol. 
CH 8 OH + two mols. C 6 H 8 . 

t o Gms. HgCU per 100 

* ' Gms. Sat. Sol. 



30 

37 



4 .8 
17- 1 
18 
18.4 



SOLUBILITY OF MERCURIC CHLORIDE IN BENZENE, IN DICHLORETHANE 
AND IN ETHYLACETATE AT DIFFERENT TEMPERATURES. 

(Dukelski, 1907.) 



In C 6 H 6 . 
fo Gms. HgClj per 
* ' 100 Gms. Sat. Sol. 

6.5 O.26 


In C S H<C1*. 

{ * Gms. HgClt per 
1 100 Gms. Sat. Sol. 

o 1.33 


In CH 3 COOCzH 6 . 

f o Oms. HjrClj per 
* ' 100 Gms. Sat. Sol. 

o 22.9 


18 


0.53 


12-5 


i .55 


6-5 


22.7 


34-i 


0.64 


25-3 


i .73 


26.1 


22.8 


54-i 


1.02 


33 


2.05 


3^5 


23-5 


69 


x -39 


45-9 


2 .42 


45-3 


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, 1907.) 



11 O. J.YA1ALU1C \Ji UUC 111U1. 

CeHe 4- one mol. 


Ail a, iri.iA.LUic: Ul UHC lllUi. 

CHCla -f one mol. 


AH a. iviiAtui t: UJL unc inui 

CCU H- two mols. 


CH S COOC 2 H 6 . 


CH,COOC 2 H 6 . 


CH 3 COOC 2 H 6 . 


xo Gms. HgClj per 
100 Gms. Sat. Sol. 


t Gms. HgCU per 
100 Gms. Sat. Sol. 


,., Gms. HgClj per 
1 ' 100 Gms. Sat. Sol. 


o 9.62 


o 3-34 


o 9.24 


6.5 9.62 


26.1 4.07 


10.3 9.05 


25.7 9.78 


36.1 4.78 


25-7 9-32 


27.6 9.98 


46 5-38 


27.6 .9.50 


35-5 I0 -Si 


48.5 5.10 


38.5 9.89 


45-3 13-^9 




45-3 ii-?o 



635 HYDRARGYRUM 

SOLUBILITY OF MERCURIC CHLORIDE IN ETHYL ACETATE AND IN 

ACETONE. 

(Etard, 1894; von Laszcynski, 1894; Krug and McElroy, 1892; Linebarger, 1894; Aten, 1905-06.) 

NOTE. The results obtained ]by the above-named investigators were calcu- 
lated to a common basis and plotted on cross-section paper. The variations 
which were noted could not be satisfactorily harmonized, consequently all the 
results are included in the following table: 

SOLUBILITY. 



In Ethyl Acetate. 
Grams HgClg per TOO Grams Solution. 



In Acetone. 

Gms. HgCfe per TOO Cms. Solution. 



* . t 
Laszcynski. 


Aten. Linebarger. 


Etard. K and McE. Laszcynski. Aten. Etard. 


10 


. . 




23 


-O 




. 


40 


... ... 


44.0* 


57- 


o 


O 


22. 


,0 


23 


-2 


32- 


o 


40 


49.7 


43 -o * 


61. 


7 


+ 10 


22 


.2 


23 


5 


32- 


5 


40 


52.0 


51.0 *-58-9 t 


61. 


7 


20 


22 


.5 


23 


4 


32- 


7 


40 


54 


58.5 t 


61. 


7 


25 


22 


-7 


23 


5 


33 





40 


37-4 55-2 


58. 2 t 


61. 


7 


30 


23.0 


33 


.2 


40 






61. 


7 


40 


23 


5 






33 


5 


40 


... ... 




61. 


7 


50 


24 


.0 


. , 




33 


5 


41 


... ... 




61. 


7 


60 


24 


7 










42-5 


... * 


. . . 


61. 


7 


80 


26 


.0 








. 


45-2 


... ... 




61. 


7 


IOO 












. 


48.0 


... ... 






. 


120 






. 






. 


50.8 


... 






. 



Cl 



(*) Solid phase HgCl2(CH 8 ) 3 CO. 



(t) Solid Phase HgClj. 



100 gms. absolute acetone dissolve 143 gms. HgCla at 18. 



(Naumann, 1904.) 



100 gtns. sat. solution of HgCl 2 in Acetone contain 54.9 gms. HgCl 2 
at 25. (Zapata y Zapata, 1930. I 

100 gms. ethyl acetate (dig. = 0.8995) dissolve 48.8 gms. HgClj at x8. 

(Naumann, 1910.) 

100 gms. methyl acetate (d^ = 0.935) dissolve 42.6 gms. HgCI 2 at 18. 

(Naumann, 1909.) 



SOLUBILITY OF MERCURIC CHLORIDE IN SEVERAL SOLVENTS. 

(Arctowski. 1894; von Laszcynski, 1894; Sulc, 1900.) 



In Carbon Bisul- 
phide (A.). 

Gms. HgCl 2 
t. per ioo Gms. 

Solution. 



IO 

O 

10 

15 
20 

25 



0-010 

0.018 
0.026 

0.032 
0.042 

0-053 
0.063 



In Benzene 


In Several Solvents 


(von L.). 


at 18-20 (S.). 


Gms. HgCla 


Gms. HgCla 


t. per ioo Gms. 


Solvent. per ioo Gms. 


Solution. 


Solvent. 


15 0-537 


CHBr 3 0.486 


41 0.616 


CHC1 3 0.106 


55 0.843 


CC1 4 0.002 


84 1-769 


C 2 H 5 Br 2.010 




C 2 H 4 Br 2 1.530 



Hg HYDRARGYRUM 636 

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 3 COCH 3 + C 6 H 6 . 



In Mixtures of 
(C 2 H 5 ) 2 + CHC1 3 . 



In Mixtures of 
CH 3 COOC 2 H 6 + C 6 H. 



Cms. CH 3 COCH 3 Cms. HRCI 2 
per 100 Grns. per too Gins. 
Mixture. Mixed Solvent. 


Gms. CHC1 3 
per loo Gms. 
Mixture. 


Gms. HgCl 2 Gms. CHsCOOCjHj Gms. HgCU 
per too Gms. per 100 Gms. per 100 Gms. 
Mixed Solvent. Mixture. Mixed Solvent. 


IOO 


140 


O 


6.95 


ICO 


49-3 


90 


117 


IO 


5.85 


90 


26 


80 


96.5 


2O 


4-73 


80 


22.1 


70 


77 


30 


3-70 


70 


18.1 


60 


60 


40 


2.80 


60 


14.2 


5 


45 


50 


2.IO 


50 


II 


40 


3i-4 


60 


1.48 


40 


8 


30 


20 


70 


o-95 


30 


5-4 


2O 


10.7 


80 


0.657 


20 


3-i 


IO 


3-9 


90 


0.328 


IO 


1.6 





0.66 


IOO 


0.128 


O 


0.66 



Cl 



SOLUBILITY OF MERCURIC CHLORIDE IN BENZENE. 

(Average curve from results of Linebarger, 1895; Sherrill, 1903; and Marden and Dover, 1917,) 



O 
IO 
2O 



Gms. HgClo 
roo Gms. Cj 

0.2O 



0.56 



25 
3 
40 



Gms. HgCl 2 per 
100 Gms. QHt. 

0.64 
0.71 
0.84 



SOLUBILITY OF MERCURIC CHLORIDE IN ABSOLUTE ETHYL ETHER. 

(Etard, 1894; Laszcynski, 1894; Kohler, 1879.) 



i. 


Gms. HgCU per 
ioo Gms. Solution. 


f. 


Gms. HgCI 2 per 
ioo Gms. Solution. 


t*. 


Gms. HgCIj per 
ioo Gms. Solution. 


20 


6 


60 


6 


90 


7-5 


o 


6 


70 


6.4 


IOO 


8 


20 


6 


80 


7 


no 


8-5 



SOLUBILITY OF MERCURIC CHLORIDE IN CHLORINATED HYDROCARBONS AT* 25 

(Hoffmann, Kirmreuther and Thai, 1910.) 



Solvent. 



Gms. 
Formula. ^per So , vent 

Solvent. 

Ethylene Chloride CH 2 C1.CH 2 C1 i . 2 29 Dichlorethylene 

Tetrachiorethane C^BkCl* 0.090 Trichlorethylene 

Chloroform CHCls o.ioi Tetrachlorethylene 

Pentachlorethane 



Formula. 



Carbontetrachloride CClI 



Gms. 
Hgdtper 
loo Gms. 
Solvent. 

CHC1.CHC1 0.114 
CHC1.CC1 2 0.0274 
CC1 2 .CC1 2 0.0072 



trace 



ioo gms. 95% formic acid dissolve 2.1 gm. HgCl 2 at 19. (Aschan, 1913.) 

ioo gms. 95% formic acid dissolve 0.02 gm. Hg 2 Cl 2 at 16.5. 

ioo cc. anhydrous hydrazine dissolve I gm. HgCb with decomp. at room temp. 

(Welsh and Broderson, 1915.) 
ioo cc. anhydrous hydrazine dissolve I gm. Hg 2 Cl2 with decomp. at room temp. 

(Welsh and Broderson, 1915.) 

IOO gms. glycerol dissolve 80 gms. HgCl 2 at 25. (Moles and Marquina, 1914.) 

ioo gms. glycerol dissolve 8 gms. HgCli ? Hg 2 Cl 2 at 15-16. (Ossendowski, 1907.) 
ioo gms. anhydrous lanolin (m. pt. about 46) dissolve 1.55 gms. HgCl 2 at 45. 

M gms. 



ioo gms. sat. solution of HgCl in Ethyl Ether contain 
(Richard, i| a 6.) 



HgCl 2 at about 20. 



637 HYDRARGYRUM 

SOLUBILITY OF MERCURIC CHLORIDE IN PYRIDINE. 

(McBride, tgio.) 

The determinations at the lower temperatures were made by stirring an excess 
of HgCla with pyridine and analyzing the sat. solution. Those at the higher tem- 
peratures were made by the synthetic method. 



Hg 



Cms. 




t . HgCl s per 
100 Cms. 


Solid Phase. 


Sat. Sol. 




32.6 2.76 


HgClj.aC 6 HN 


-21.75 7-86 


" 


0.02 13.14 


" 


12.58 17.34 


" 


18.78 19.78 


" 


27.23 22.65 


" 


31.05 24.46 


" 


40 .90 29 . 29 


" 


50.10 34.94 





60.03 40-36 


" 


70.15 46.44 





76 


" + HgClj.QHjN 


80.02 51.52 


HgCl 2 .2C 6 H 6 N (unstable) 


89 56.45 


" " 


94.1 60.09 


u K 



94-7 
74-7 
83-5 
90.4 

97 

100.5 
104.2 
107 
106.2 

95-2 
106.4 
109.8 
114 
124.2 
145-5 



Cms. 
HgCUper 
100 Gms. 
Sat. Sol. 
60.72 
48.38 
50-53 
53-41 
56.45 
57.84 
60.72 
63.06 

60.77 
61.93 
62.58 
63.18 

65 
69.66 



Solid Phase. 

HgCl 2 .2C 6 H 6 N+ 3 HgCl,.2QH i N 
HgCl 2 .C 6 H s N(unstuble) 
(stable; 



(unstable) 
+3HgCl 4 . 2 C 6 H 6 N 
3HgCl 2 .2C 6 H 6 N (unstable:) 
(stable) 



Data for this system are also given by Staronka (1910). 

Data for the solubility of HgCl 2 .2C 6 H 6 N and of Hg(N03) 2 .2C 6 H 6 N.2H 2 O in 
aqueous solution of pyridine at i8.i are given by Stromholm (1908). 

Data for the solubility of diamine mercuric chloride, (NH 3 )2HgCl 2 NHjHgCl, 
in aqueous solutions of ammonia at 17.5 are given by Stromholm (1908). 



Cl 



SOLUBILITY OF MERCURIC CHLORIDE AND OF DOUBLE MERCURIC AND 
TETRA METHYL AMINE CHLORIDE (CH 3 ) 4 NC1.6HgCl 2 IN AQ. ETHER 

AT 1 7. (Stro'mholm J. pr. Ch. [2] 66, 443, '02; 2. physik. Chem. 44, 64, '03.) 



Molecular Concentration per Liter. 



Grams per Liter of Solution. 



H 2 0. 


HgCl 2 (*). 


HgCl 2 (t). 


H 2 O. 


HgCl 2 (*). 


HgCI 2 (f). 


o.o 


O^SIS 


0.0342 


O 


41 -l6 


9.26 


0.0656 


0-1795 


o .0428 


1.18 


48.64 


II. 60 


0.1311 


o . 2069 


0-0516 


2.36 


56.08 


14.00 


0.1956 


0-2339 


o . 0603 


3-52 


63-38 


16.34 


0.2611 


o . 2489 


0.0690 


4-70 


7O.l6 


18.70 


0.3267 


o . 2849 


0.0779 


5-88 


77.20 


21 .IO 


0.3922 


0.3100 


0.0866 


7.06 


84.02 


23.48 



(*) Results in this column are for solutions in contact with the Solid Phase HgQ 2 . (t) Results n 
this column are for solutions in contact with the Solid Phase (CH3) 4 NC1.6HgCl2- 



SOLUBILITY OF MERCURIC CHLORIDE AND OF DOUBLE MERCURIC AND 
XETRA METHYL AMINE CHLORIDE IN ALCOHOL-ETHER SOLUTIONS 

AT 17. (StrSmholm.) 

Grams C 2 H 5 OH per Liter. Grams HgCl 2 (*) per Liter. Grams HgCl 2 (t) per Liter. 

o.o 41.16 9.26 

4.58 50.00 11.87 

9.16 58.76 14.38 

13.74 66.96 16.90 



Hg HYDRARGYRUM 



638 



Cl 



SOLUBILITY OF DOUBLE MERCURIC CHLORIDES IN AQUEOUS AND PURE 
ETHER AT 16.6. 

(Stromholm, 1902, 1903.) 
Mol. Cone, of HgClj per Liter of: Gms. HgCl 2 per Liter of: 



Pure Aq. Aq. Aq. Pure Aq. Aq. Aq. 

Ether. Ether Ether- Ether Ether. Ether Ether Ether 

(i). (2). (3)- % (4). (5). (6). 

0.1515 0.2387 0.2647 0.3196 41.04 64.69 71:71 86.58 

0.0673 - I1 S7 0.1293 0.1617 18.23 31.41 35-S 43-79 

0.0404 0.0720 0.0835 0.1034 10.95 19.51 22.61 28.01 

0.0342 ... 0.0706 ... 9.26 ... 19.10 ... 

0.0264 0.0568 ... 7.14 ... 15.39 

0.0209 0.0400 0.0460 0.0594 5.66 10.83 12.48 16.10 

0.0063 ... 0.0144 ... 1.70 ... 3.90 ... 
(i) containing 0.21055 moi. H 2 O per liter. (2) 0.2756 mol. H 2 O per liter. 



Solid Phase. 



HgCl* 



(CH3) 4 NC1.6HgCl 2 
(C 2 H 6 ) 3 SC1.6HgClj 



(CH,) 2 .H 2 NC1.2HgClj 

(3) 0.421 mbl. Hop per liter. 



. . . . . 

(4) containing 3.79 gms. H 2 O per liter. (5) 4.97 gms. H 2 O per liter. (6) 7.59 gms. H 2 per liter. 

SOLUBILITY OF MIXTURES OF MERCURIC AND POTASSIUM CHLORIDES AT 25 IN: 



Absolute Alcohol. (Foote, 1910.) 



Acetone. (Foote, 1910.) 



Gms. per 100 Gms. 
Sat. Solution. 

' KC1. ^ 
0.21 
0.28 
0.22 
0.28 
0.25 
0.17 
0.38 



33.69 

33.80 

24.84 

6.21 

1.65 

1.57 

1.03 



Solid Phase. 

Hgd|+sKa.6HgClt.2C,H,OH 
" " 

5KC1.6HgCl 2 . 2 Q>H 6 OH 

" 
5KCl.GHgCl 2 .2C J H 6 OH+KCl 



Gms. per 100 Gms. 
Sat. Solution. 

* 



Solid Phase. 



KC1. 
1.27 
1.39 
2.58 
2.78 
2.93 
2.52 
3.34 
2.92 



HgClo. * 

61.87 

60.68 

55.85 

54.41 

48.13 

18.04 

13.26 

II 



KCl.sHgCl 2 .(CHa) 2 CO 



-4-5-6.2 



5.6.2 



+K.C1 



5.6.2 = 5KC1.6HgCl 2 .2(CH 3 ) 2 CO. 



100 gms. of sat. abs. alcohol solution of HgQ 2 + NaCl contain 46.85 gms. 
HgCla and 3.01 gms. NaCl at 25. (Foote, 1910.) 

SOLUBILITY OP MERCURIC CHLORIDE AND SODIUM CHLORIDE IN ETHYL 

ACETATE AT 40. 

(Linebarger Am. Ch. J. 16, 214, '94.) 



Mols. per TOO Mols. 
Acetate. 


Gms. per 100 Gms. 
Acetate. 


Gms. per 100 Gms. 
Solution. 


Solid 
Phase. 


flaCl. 


HgCl 2 . 


NaCl. 


H g ci 2 : 


NaCl. 


H g ci 2 : 




0.8 


12-9 


o-S3 


39-7 


o-53 


28.4 


HgCla 


*-3 


12-4 


I -S3 


38-15 


1 -Si 


27.61 





4-3 


16.4 


2.8 S 


50-44 


2.78 


33-54 


< 


9.1 


22.8 S 


6.05 


86.14 


5.60 


46.28 


i 


18.5 


34-9 


12 .29 


107.4 


10.95 


S 1 ^ 





20 .0 


40.0 


13.29 


123.0 


n-73 


55-i8 


HgCia-f Na< 



The double salt (HgCl 2 ) 2 .NaCl is formed under proper conditions. 



639 HYDRARGYRUM 

FREEZING-POINT DATA ARE GIVEN FOR THE FOLLOWING MIXTURES, 



H 



Mercuric Chloride + Mercuric Iodide 



Mercuric Sulfate 
Lead Chloride 
Ammonium Chloride 
Silver Nitrate 
Thallium Nitrate 
Thallium Sulfate 
Selenium 
Antimony Chloride 

Sulfur 
Nitrobenzene 



" " Q ITJ and 2 Nitrotoluene 

" " * Urethan 

11 " *> " + Nitronaphthalene 

" " + " + JbNitrotoluene 

" " + oc Nitronaphthalene 

11 " r jo Nitranisole 

MERCUROUS Per CHLORATE Hg g (C10 4 ) 2 

SOLUBILITY OF MERCUROUS PBR 

(Newbery, 1936.) 



(Padoa and Tibaldi, 1903; 

Losana, 1926; Bergmann 

and Gonke', 1926. ) 
(Paic, 1930, 1933.) 
(Van Drielj 1935. ) 
(JSlnecke, 1923.) 
(Bergmann, 1926. I 

(Waskresenskaja, 1929. ) 
(Olivarij 1909.) 
(Kendall, Crittenden and 

Miller, 1923,) 
(Olivari, 1909.) 
(Mascarelli, 1906; 

Mascarelli and Ascoli , 

1907. ) 

( Mascarelli , 1906, 1907, 

1909. ) 

(Mascarelli, 1908, 1909.) 

( " 19069 1907.) 

( " 1908.) 

( " 1906, 1907. ) 

( " 1 906 . ) 



CHLORATE IN WATER. 



Cic 



o 


Oms. Hg 2 (C!0 4 ) 2 per 




100 Sns. H 2 


20 


215 H 





282 


i- 8 


315 


17 


355 


20(d 


= 2.960)368 


30 


420 


35 


450 


36 


4<35 



Solid 
Phase 



37 
38 
40 
50 
60 
70 
78 



Oros. 
100 



455 
455 
457 
480 
500 
516 
536 
580 



Solid 
Phase 



H?(C10 4 ) 



SOLUBILITY OP MBRCUROIJS PER CHLORATE IN AQUEOUS 
SOLUTIONS OF PERCHLORIC ACID AT 21. 

(Newbery, 1936.) 



Mols. free HC10 4 
per 100 gms. H g O 

0.10 
0.38 
0.46 
1.27 
1.29 



Qms. 
per 100 



375 

300 

280 
21.2 
13.7 



HgO 



Solid 
Phase 



The total gm. mols. of HCIO^ in the above solutions is nearly con- 
stant' hence each added gm. mol. of HC10 4 precipitate approximately 
one gm. mol. equivalent of the salt.. 



Hg HYDRARGYRUM 64O 

MERCUROUS CHROMATE Hg 2 Cr0 4 

Tiie Solubility Product of Mercurous Chromate in Water at 25 is 
2.0 x io" 9 as quoted from Immerwahr by Brodsky, 1929. 

MERCUROUS Phospho FLUORIDE IIggP0 3 P 

One liter sat. solution of Mercury Phospho Fluoride in Water contains 

about 0.0005 gm. mols. (= 0.025 f*m.) ^? 2 ^s^ at 20 * (^ange, 1929.) 



MERCUROUS IODIDE U? ? I ? 

SOLUBILITY OF MERCUROUS IODIDE IN WATER AT 25. (Sherriii, 1903.) 

One liter sat. solution contains 2 X io~ 7 gms. Hg 2 l2, determined by indirect 
method. 

Data for the solubility of mercurous iodide in aq. KI solutions at 25 are also 
given by Sherriii. 

The Solubility Product of Mercurous Iodide in Water, calculated from 
measurements of the F/.M.F. of a chain electroded by Brodsky, 1929, is as 
follows: 

t Solubility Product 

10.8 2.01 X 10 ~ 20 

14.9 5.10 x io" ?0 
19.2 10.5 x io" 20 
25.0 49-5 * io~ 20 

26.5 74-2 X 10~ 20 

MERCURIC IODIDE HgI 2 

SOLUBILITY OP MERCURIC IODIDE IN WATER. 

t Ctas. Hglg per liter Authority 

17.5 0.040 (Bourgoin, 1884.) 

22. 0.054 (Rohland, 1898.) 

22,5 o.ooi (Naude, 1927.) 

25. 0.059 (Morse, 1902.) 

SOLUBILITY OP MBRCURIC IODIDE IN WATBR AT TEMPERATURES 
ABOVE 100 DETERMINED BY THE SYNTHETIC METHOD. 

(Benratti, QJedebo, Schl f fera and VArnderllch, 1937.) 

At 11.5 percent concentration of HgI 2 and temperature of 241 the 
mixture separates into two liquid layers, composed of a yellow solution 
and a wine red melt. These two layers mutually dissolve with rising 
temperature. At 77 percent HgI 2 and 338* the solution an4 melt become 
identical and mix in all proportions above that temperature. 



.0 


Qns. Hgl, 


? per Solid 


r o 


Ctas. Hgl. 


? per 


r O 


ftna. Hgl ? per 


100 gms. aat. sol. Phase 


t 


100 8s. Bt 


it. sol. 


t 


100 gms. sat. 


sol. 


196 


3- 


7 tfgtg 


243 


12. 





328 


54.4 




229 


9. 


4 " 


257 


1^. 


7 


336 


68.0 




241 


11. 


5 


272 


18. 


7 


338 


75-0 




241 


98. 





295 


27. 


5 


336 


82.7 




255 


100. 


" 


314 


41. 





322 


90.5 










326 


49- 


7 


262 


97-4 





641 HYDRARGYRUM 

SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS SOLUTIONS AT 25. 

(Hens and Paul, 1913.) 



In Aq. BaI 2 . 

Mols. per Liter. 


In Aq. CaI 2 . 
Mols. per Liter. 


In Aq. Nal. 

Mols. per Liter. 


In Aq. SrI 2 . 

Mols. per Liter. 


Bal s . 
0.099 
0.748 
0.978 
I.S08 


HgI 2 . 
0.059 
0.742 
0.897 
1.462 


'CaI 2 . 
0.053 
0.252 
0.468 
1-799 


HgI 2 . ' 
0.050 
6.261 
0.440 
1.706 


Nal. 
0.794 

1.385 
2.225 


HgI 2 .' 
0.412 
0.622 
0-945 


SrI 2 . 
0.254 
0-355 
0-539 
0.608 


H g i 2 : 

0.212 
0.320 
0.582 
0.694 



SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS SOLUTIONS OF POTASSIUM 

IODIDE AT 25. (SherrUl, 1903; Herzand Paul, 1913.) 
Mols. per Liter. Gms. per Liter. Mols. per Liter. Cms. per Liter. 



' KI. 


HgI 2 / 


'KL 


Hgl,. ' 


KL 


HgI 2 . 


' KL 


HgI 2 . 


0.05 


0.025 


8-3 


11.4 


I 


0.50 


166 


227.2 


O.IO 


0.05 


16.6 


22.7 


1-5 


0.75 


249 


340.8 


O.20 


O.IO 


33-2 


45-4 


2 


I 


332 


454-5 


0.50 


0.25 


83 


113.6 


2-5 


1.25 


415 


578 



Data for the distribution of mercuric iodide between aq. KI solutions and 
benzene at 25 are given by Sherrill, 1903. 

EQUILIBRIUM IN THE TERNARY SYSTEM MERCURIC IODIDE, POTASSIUM 
IODIDE, WATER AT 20 AND 30. (i)unningham 1914.} 

Results at 20. Results at 30. 

Gms. per 100 Gms. Sat. Sol. Gms. per 100 Gms. Sat. Sol. 

, A N Solid Phase. . * > Solid Phase- 

KL HgU. KI. Hgl,. 

50.9 19.3 KI 60.6 ... KI 

44-4 3 2 -4 " 40 S3 "+KHgi, 

39 48 " 39.6 52.7 KHgj, 

37-4 53-6 "+KHfl, 40 52.2 

37-8 52.6 KHgi 3 40.2 51.2 

35-1 52.2 " 39.3 50.3 

35.5 51 2 KHgI,.H 2 33.7 49.8 

26.7 50.3 "+HI S 33 52 

26.6 49.4 Hgl, 31.4. 51.7 KHgI,.H,0 

23.7 40.2 " 29.1 52.2 
14.9 22.5 

EQUILIBRIUM IK THB SYSTEM MERCURIC IODIDE, POTASSIUM IODIDE AND WATER 

AT 22.5. 
(Naude, 1927.) 

The solutions were analyzed by reducing the mercury and converting the 
iodine to KI by adding KOH and C H g OH and warming. The total KI in the 
filtrate from the H? was titrated with standard solutions of AgNO, and 
KSCN. 

Qna. per 100 One. per 100 Ana. per 100 

0ns. sat. sol. Solld 9.8. sat. 801. Sollcl 0ns. aac. aol. Solld 

/ :j ^ nut ^ Phaac 



o.o o.oi HgI 2 29.18 49.18 1.1. li 34.84 5i53 1-1 

1.95 2.02 " 31.18 49.28 " 36.45 51.28 KI 

16.16 10.96 " 32.68 49.15 " 36.69 50.01 " 

24.60 45.06 " 33.37 49.67 " 37.6i 47.04 " 

24.57 46.93 " 33.92 50.10 " 40.41 37.41 " 
25.10 49.13 " * i.i.ii33.79 51.13 " 49.60 18.37 " 

27.58 49.o6 1.1. li 34.04 51-74 i.l 58.33 l-6o " 
28.44 48.97 " 34-92 51-58 " 59.20 0.0 " 

1.1. li = HgI 2 .KI.iiH 2 0; 1.1 = HgI 2 .KI 



Hg HYDRARGYRUM 



642 



MERCURIC IODIDE Hgl g 

EQUILIBRIUM IN THE SYSTEM MERCURIC IODIDE POTASSIUM 
IODIDE AND WATER AT SEVERAL TEMPERATURES. 

(Pernot, 1926. 1927, 1931.) 

The samples were analyzed by separating the Hfl g from the KI by 
sublimation in a glass tube which could subsequently be cut and the 
amount of each component determined by weighing. The accuracy of the 
results of Cunningham, 191 <i, is questioned. 



Results at o 



Results at 10 



Results at 20 



fins, per 100 


ftos. per 100 


gms. sat, sol. Soll<1 


gms. sat. sol. Solld 


-H5^ 


f> Phase 


'Tgir" 


syN Phase 

M 


19.1 


13.3 HgI 2 


19.6 


12.0 M?Ip 


32.7 


21.1 " 


34.9 


22.0 " 


39-9 


25.0 " 


41.7 


25.5 " 


41.8 


26.7 1,1.1 


44.8 


27.0 1.1.1 


43-3 


29.7 


46.6 


30.7 " 


45.5 


32.1 


48.1 


33.7 " 


47.8 


34.8 


49-3 


35-7 


50.2 


37-5 " 


50.8 


37.5 


47.5 


38.1 KI 


50.9 


37.9 " + KI 


43.7 


38.9 


48. i 


38.3 KI 


39.2 


40.0 " 


46.5 


38.6 " 


34.0 


41 9 " 


44*7 


39-0 


28.4 


43-9 " 


38.2 


41.2 " 


24.1 


45.6 


35-7 


42.3 " 


19.3 


47. M " 






15.6 


49-2 " 








Results at 34 


Results at 56 


3.1 


2.2 Hglg 


4.1 


3.2 Hgl 


20.3 


12. 9 " 


27.4 


16.6 " 


47.4 


26.2 


46.1 


25.0 " 


53-4 


27.7 "+1.1. 


i 57-1 


27.5 " 


52. n 


29.3 1.1.1 


57-4 


28.8 1.1.1 


51.9 


30.7 " 


56.4 


30.2 " 




34.4 " " 


54.9 


32.8 " 


52.5 


37.6 " + .K1 


54-2 


37.5 " + KI 


49.8 


38.3 KI 


53-0 


37.9 KI 


46.1 


39-3 


46.6 


39.8 " 


42.3 


40.5 " 


41.2 


42.0 " 


33.7 


44.2 " 


24-7 


49.4 " 


15.6 


52.9 


12.8 


56.1 " 






3.9 


61.4 " 



CfclS. 


per 100 


gms. sat. sol. ^Ua 


' Hgl ? 


s j^^ p ha 3 e 


10.3 


74 ^2 


24-3 


16.2 " 


34.7 


21.3 " 


41-3 


24 . 6 " 


48.2 


27.3 " + 1.1 .1 


48.0 


29.0 1.1.1 


48.7 


31.3 


49.2 


33-4 


49-9 


34-9 


50.9 


36.8 " 


50.0 


37.9 KI 


45-3 


39.1 


31.0 


44-4 


16.7 


50.6 " 


8.7 


53.8 " 




Results at 8o : '' 


1 .2 


0.6 HgI 2 


19.1 


11.3 " 


40.8 


20.9 " 


54.3 


2^.6 " 


65.0 


26.2 "*!. 1.1 


C 3 .2 


27-6 1.1.1 


6l . 1 


29.4 " 


58.2 


33-0 " 


57.5 


36.2 " + KI 


50.7 


36.6 KI 


46.5 


40.4 " 


28.9 


48.3 " 


15-5 


56.2 " 


8.0 


60.8 " 



1.1,1 = H?I ? .KI.H 0. No evidence was obtained of the existance of 
the compound tJglg.Kl. 



l,y 
it* fi ''VSTIIH MKKn*iw lt*t$iii 

AW ii KTHtl, Ai,fftf4ii Af fii* 1 . 

ft't>fWt |,H!*'I 



H . 1 t*' f J * 

J 1 . ft 
1 |J ' ? 

s.rt ju.-> * " * *;?.t iv.u (t *J ,.U>^ ^ 

^j.7 ^ " ''^- |j - 11 *' < 

St ,? ,i.< .^ " % <.-* / ! I 

M.t ( ,7 

MJ. i jCi . i M 

ill, 7 ^***l 



ANU iKttl'fJttmtfi It'Ufit^i Af Jts" 1 . 



KMt,, *l t ' |t|i< 

n,i rt,i| tU*! ? ii',,.,- 

'!.*) M.I* ** ?*li 

t.^.rt I M *' ^ii,, 

till . | tv.fc " |J ^>. 

li^i . *| ^*l . i| " I . 1 I . A * ' ** M ' 

*< .V J*> 1 t , I . I ' I "1^*1 t i " 



4l*i* jftV**" |*f rf" ifiif i * t*l *^-* **4Uli*tli* 5*' vrl'.n* 

VJ , I J , t'l | V i . $ 1 t, if /*, | * * r ! *, ! " '- *"^ 

4'l *Ji*f |*I|f \* \ in *,sf,%tltft Ju,v v f,ir* , |% tl'i'ti* ? I ^r 

*,iJf*i. 1 / -ra t * 1 1 f f r-f-rnt *l ? H |-i if <f it it > -uil u it i a* i I 
!*l HtAf tit i *on<* uiiuun* I I '^, * f *.* f 1, 1 ti.jjr* nA t 
i ] '}| ty . Kl , ^ * In .1 *i Ht* <Binii/ j 4, $ ''! 1 

M *4 * ilt<f 111. - I <! I t If */**' 1^^ 'si I" / ; , ^H 1*11 i!*4J 

if 44** * til m* ,il j ' . tJt* .1% t*ir !i ! ! " -s*'' f^'iti 1 



* pl'i. nll 'tt I ill I I, 
41 */ . I *4|t*fp| ) - + 



Hg HYDRARGYRUM *44 

EQUILIBRIUM IN THE TERNARY SYSTEM MERCURIC IODIDE, POTASSIUM 

IODIDE, ETHYL ETHER AT 20. (Dunningham, 1914.) 
Two liquid layers with compositions as follows, are formed: 
Gms. par ioo Gms. Upper Layer. Gms. per 100 Gms. Lower Layer. ^ 



HgI 2 . 
2.8 



KL 



None 



Kl. 
I.I 

i.i 2.4 17-6 S3- 2 

0.8 2.5 16.5 56- 1 

None 17 58-2 

Data are also given for the four component system, HgI 2 -f Kl + (C 2 Hs)20 -f 

H*O at 20. The results are of special interest since 3 liquid layers are formed. 



KI+KHgI 3 

KHgl, 

Hgl, 

KHgI,+HgI 2 



SOLUBILITY OP MERCURIC IODIDE IN AQUEOUS ETHYL ALCOHOL: 



At 1 8. 

(Bourgoin.) 


At 25. 

(Herz and Knoch Z. anorg. Ch. 45, 266, '05.) 


r*" 

Solvent. 


Cms. Hgl t 
per Liter. 


Wt.% Alcohol 
in Solvent. 


Hgl* per ioo cc. Solution. 


Sp. Or. of 
iolutions 25/4 


Alillimols. 


Grams. 


Abs. Alcohol 


11.86 


IOO 


3 .86 


1-754 


0.8033 


H 2 O 4-8o% 90 Ale. 
1^0+10% 90 Ale. 


2.857 
0.086 


95-82 
92-44 
86-74 


2.56 
1.92 
1.38 


i .162 
0.873 
0.623 


0.8095 
0.8154 
0.8300 






78-75 


0-935 


0.425 


0.8405 






67.63 


0-45 


0.204 


0.8721 



SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS METHYL ALCOHOL AND IN 
AQUEOUS ETHYL ACETATE AT 25. (Herz and Anders, 1907.) 

In Aq. Methyl Alcohol. 

Wt.% 
CHjOHin 
Solvent. 

47.06 0.9186 0.9187 0.044 

64 o.SSoo 0.8834 0.158 

0-445 
2.590 



78.05 
IOO 



<?of 
Solvent. 
0.9186 
0.8SOO 
0.8489 
0.7879 



Sat. Sol. 
0.9187 
0.8834 
0.8519 
0.8155 



Gms. HgI 2 

per ioo cc. 

Sat. Sol. 



In Aq. Ethyl Acetate. 
Wt. % CH r <v of Oms. Hgl, 

COOC 2 Hs 

in Solvent. 



96.74 
IOO 



Sat. Sol. 

0-9973 
0.9063 
0.90II 



pcnopcc. 



Sat. Sol 
0.013 
1.8 7 
1.09 



ioo gms. sat. solution in 95% alcohol (Jis = 0,8126) contain 0.72 gm. Hgl 




at o, 1.06 grns. at 25 and 2.15 gms. at 50. 



(Remders, i9cx>.) 



MEKCURY IODIDE (ic) HgI 2 . 

SOLUBILITY OF MERCURIC IODIDE IN METHYLAL (H CH (O CH 3 ) 2 ). 
( Boiirgoin, 1924. ) 

The methylal was purified by distillation over sodium. At the lower temperatures 
the solutions were saturated by constant agitation. At the higher temperatures 
the synthetic method was used. 

Gms. Hgl, Solid 

per 100 gms. sat. sol. Phase. f- 

.... 3.8t HgU(red) 74... 

4-7 77 

.... 4.19 81 

4.56 > 1*3 

i*25 (tr. pt.). 

136.5 

1 66 



t". 
20 

25 

3o 
53 
63 
67 



Cms. Ilgls 
too gms. sat. sol. 



5.12 

5.32 
5.56 



5.8o 
5.93 

6.0D 

7.89 

7:9<> 

8.00 
8.14 



Solid 
Phase. 

Hgl, (red) 



-HlTg I, (yellow) 

HgI 2 (yellow) 



645 

SOLUBILITY OF MERCURIC IODIDE IN ALCOHOLS. 



HYDRARGYRUM 



Alcohol. 


Formula. 


t. 


Sp. Gr. of v 
Solution. 


_UU3. XJLKJ.2 \Jm 

zoo Cms. Observer. 
Alcohol. 


Methvl 


CHaOH 


15-20 


0.799 


3 . 24 (Rohland.) 


t( 


a 


19 




3 . 7 (Timofeiew.) 


it 


it 


iQ-5 




3.16 (de Bruyn.) 


n 


it 


23 




3 . 98 (Beckmann.) 


a 


a 


66 (b. pt.) 


. . . 


6.512 (Sulc.) 


Ethyl 


C 2 H 6 OH 


15-20 


0.810 


1 . 42 (Rohland.) 


i 


a 


18 


. . . 


1 . 48 (Bourgoin.) 


i 


a 


19 


. . 


1 . 86 (Timofeiew.) 


t 


11 


19.5 




2 . 09 (de Bruyn.) 


t 


(t 


25 


0.803 


2.19 (Here and Knoch.) 


i 


tt 


78 (b. pt,) 




4.325 (Sulc.) 


Propyl 


C3H 7 OH 


15-20 


0.816 


0.826 (Rohland.) 


u 


tt 


19 


... 


1.25 (Timofeiew.) 


Amyl 


CsHnOH 


13 




. 66 (Las2cynaki.) 


u 


ti 


71 




3-66 


li 


a 


100 




5-30 


tl 


tt 


133.5 


* . . 


9-57 


Isopropyl 


(CH 3 ) 2 CH.OH 


8l (b.pt.) 


... 


2.266 (Sulc.) 


Isobutyl 


(CH 3 ) 2 CHCH 2 OH 


22.5 




0.51 (Timofeiew.) 


u 


n 


IO5-IO7 (b 


pt.) . . . 


2.433 (Sulc.) 



SOLUBILITY OF MERCURIC IODIDE IN MIXTURES OF ALCOHOLS AT 25. 

(Herz and Kuhn, 1908.) 

In CH 3 OH+C 2 H 6 OH. In C 3 H 7 OH+CH 3 OH. In C 3 H 7 OH+C 2 H6OH. 



Per cent 


,/ of Gms - Hgl * Per cent " 


r n f Gms. HgI 2 Per cent , 


i-. of Gms.Hglj 


CH,OH in 
Solvent. 


Sat. Sol. 


per ioo cc. CaHyOH in 
Sat. Sol. Solvent. 


Sat. Sol. 


per ioo cc. C 3 H 7 OH in 
Sat. Sol. Solvent. 


TT penoocc. 
Sat. Sol. H Sat.SoU 


O 


0.8038 


1. 80 


o 




0. 


8156 


3-16 


O 


O. 


8038 


I. 80 


4-37 


0.8039 


1-93 


ii, 


,11 








8.1 


0. 


8036 


1-73 


IO.40 


o . 8046 


2.08 


23- 


.80 


O. 


^155 


3-04 


17-85 


0. 


8043 


1-65 


41.02 


0.8077 


2.32 


65 


,20 








56.6 


o. 


8057 


i-55 


80.69 


0.8I3I 


2.89 


91, 


.80 





.8101 


1.69 


88.6 








84.77 


O.8l4O 


2.96 


93 


75 


o 


.8110 


1.67 


91.2 


0. 


,8099 


1.52 


91.25 


0.8146 


2.98 


96 


.60 





.8108 


1.53 


95-2 


o. 


,8108 


1.44 


IOO 


0.8156 


3.16 


100 




0, 


.8116 


1.42 


IOO 


o. 


,8ll6 


1.42 



SOLUBILITY OF MERCURIC IODIDE IN ACETONE IN ETHYL ACETATE 
AND IN BENZENE. 

(Sulc; Krug and McElroy J. Anal. Ch. 6, 186, '92; Laszcynski Ber. 27. 2285, *94-) 



In Acetone. 



In Ethyl Acetate. In Benzene. 





Gms. Hrl* 




Gms. HgI 2 




Gms. HgI 2 


t. per too Gtns. 
(CH 8 ) 2 CO. 


t. per ioo Gms. t. 
CH 8 COOC 2 H 8 . 


per ioo Gms. 


I 


2.83 


2O 


1-49 


15 


0-22 


18 


3.36 


+17-5 


1.56 


60 


0.88 


25 


2.09 (K.andMcE.) 


21 


1.64 


65 


0/95 


40 


4-73 


40 


2-53 


84 


1.24 


58 


6.07 


55 


3.19 80 (b.pt.) 0.825 (Sulc.) 


j6 (b.pt.) 3. 249 (Sulc.) 


76 


4-3 1 







74-78 (b.pt.) 4. 20 (Sulc.) 



HYDRARGYRUM 

100 gms. acetone 
benzene 
chloroform 
acetone 



ethyl acetate 



646 

dissolve 2.04 gms. Hgla at 23. 

0.25 " 
" 0.07 " 

" 2 " 

3-09 " 



(Beckmann and Stock, 1895.) 



1.47 



(red) at 25. 
(yellow) at 25. 
at 1 8. 



(Reinders, 1900.) 
(Naumann, 1910.) 



One liter sat. solution in benzene contains 2.24. gms. HgU at 25. 

(Abegg and Sherrill, 1903.) 

SOLUBILITY OF MERCURIC IODIDE IN ANILINE. 

(Pearce and Fry, 1914.) 
Solid Phase. 
C 6 H 6 NH 2 +HffI 2 .2C 6 H 6 NH 2 





Gms. Hglj 


t*. 


per 100 Gms. 




Aniline. 


-11.48* 


... c 


- 6.5 


23-35 


+ 0.4 


28.69 


17.8 


42.85 


21. 1 


47-55 


26.9 


55-47 


3 O.I 


62.05 


36,2 


75.80 


42.9 


96.49 


46. 8f 





+HgI 2 (red) 



Gms. HgT 2 
t. per 100 Gms. Solid Phase. 




Amline. 




48.8 


I28.I 


HgI 2 (red) 


6 3 .6 


163.8 


" 


70.82 


184.1 


" 


76.2 


2OI .6 


u 


95-9 


246.7 


tt 


io8f 




" +HgI 2 (yellow) 


115.7 


281.8 


Hglj (yellow) 


137.2 


285.2 


" 


181.1 


297.9 


" 


199.1 


863.2 


M 



1 Eutec. 



f TV. pt. 



Additional data on this system are also given by Staronka, 1910. 

Data for the solubility. of mercuric iodide in nitrobenzene and in p nitrotoluene, 
determined by the synthetic (sealed tube method), are given by Smits and Bak- 
horst (1915). The transition point of HgI 2 , red to yellow, was found to be at 
1.68 mol. per cent HgI 2 and 127.5 in nitrobenzene and 1.81 mol. per cent HgI 2 
and 128 in p nitrotoluene. The interesting part of the investigation is the 
characteristic prolongation of the melting line above the transition point. Similar 
data for the sojubility of mercuric iodide in nitrobenzene, m nitrotoluene, p nitro- 
toluene and in nitronaphthalene, determined by the freezing-point method, 
using a Beckmann apparatus, are given by Mascarelli (i9o6a). Observations 
on the appearance and color changes of the Hgla are given. 



SOLUBILITY OF MERCURIC IODIDE IN CARBON BISULFIDE. 

(Linebarger, 1894; Arctowski, 1894, 1895-96.) 





Gms. Hglj 




Gms. riglj 




Gms. HgI 2 


t. 


per 100 Gms. 
Solution. 


f. 


per 100 Gms. 
Solution. 


t. 


per too Gms. 
Solution. 


116 


O.OI7 


- 5 


O.I4I 


IS 


O.27I 


93 


0.023 


o 


0.173 


2O 


0.320 


86.5 


O.O24 


+ s 


O.2O7 


25 


0.382 


10 


0.107 


IO 


0.239 


30 


0.445 



One liter sat. solution of mercuric iodide in C$2 contains 3.127 gms. at ^5. 

(Dawson, iQogb). 

One liter sat. solution of mercuric iodide in CCU contains 0.170 gm. at i8 6 . 

__ (Dawson, 19096.) 

Data are also given by Dawson for the distribution of HgI 2 between aqueous 
solutions of KI and 82 at 15 and aqueous solutions of KI and CC1 4 at 18. 

100 cc. anhydrous hydrazine dissolve 69 gms, Hgl a with precipitation of Hg 
at room temp. tWelsh and Broderson. 1915.) 



647 

SOLUBILITY OF MERCURIC IODIDE IN SEVERAL 

(Sulc Z. anorg. Ch. 25, 401, *oo.) 



HYDRARGYRUM 
ORGANIC SOLVENTS, 



Solvent. 

Chloroform 

Chloroform 

Bromoform 

Tetra Chlor Methane 

Tetra Chlor Methane 

Ethyl Bromide 

Ethyl Bromide 

Ethylene Di Bromide 

Ethyl Iodide 

Ethylene Di Chloride 

Iso Butyl Chloride 

Methyl Formate 

.Ethyl Formate 

Methyl Acetate 

Acetal 

Epi Chlor Hydrine 

Hexane 



Formula. 

CHCL, 



CHBr s 

CCI 4 

CC1 4 

C 2 H 5 Br 

C 2 H 5 Br 

C 2 H<Br 2 

C 2 H 5 I 



(CH 3 ),.CHCH 2 C1 

HCOOCH 3 

HCOOC 2 H 5 

d^COOCH, 

CK,CH(OC 2 H 5 ) 2 

CH 2 .O.CH.CH 2 C1 

C,H M 



t o Gms . Hgl2 per 100 


* Gms. Solvent.. 


18-20 


O.O4O 


61 (b. pt) 


0.163 


18-20 


0.486 


18-20 


O.OO6 


75 (b- pt) 


0.094 


18-20 


0.643 


38 (b. pt) 


0-773 


18-20 


0.748 


18-20 


2.041 


85.5 (b.pt.) 


1.200 


69 


0.328 


36-38 " 


I.I66 


52-55 " 


2.ISO 


56-59 " 


2.500 


105 " 


2.000 


117 


6.II3 


67 


O.072 



SOLUBILITY 



v OF MERCURIC IODIDE IN 


ETHER AND IN METHY 


IODIDE. 




In Ether. 

(Sulc; Laszcynski.) 


In Methylene Iodide. 

(Retgers Z. anorg. Ch. 3, 253, '93.) 


M.6 Gms. Hgljt per TOO 
* Gms. (CaHa^O. 


to Gms. HgI 2 per 100 
* ' Gms. CHala. 


o 0.62 

36 0.97 

35 (b.pt) 0.47 (Sulc) 


IS 2.5 
IOO l6.6 

180 58.0 



SOLUBILITY OF MERCURIC IODIDE IN FATTY BODIES. 

(Mehu J. pharm. chim. [5] 12, 249, '85.) 

*'i 

25 
IOO 

25 
IOO 



Solvent. 

Bitter Almond Oil 
Bitter Almond Oil 
Castor Oil 
Castor Oil 



j. HgI 2 per 
ms. Solvent. 


Solvent. 


t o Gms. HgTa per 
* loo Gms. Solvent 


o-S 


Vaseline 


25 


0.025 


i-3 


Vaseline 


IOO 


O.2O 


4.0 


Poppy Oil 


25 


1.0 


20. o 


Olive Oil 


25 


0.4 


i-3 


Carbolic Acid 


IOO 


2-0 



Nut Oil loo 

loo grams oil of bitter almonds dissolve 5.0 grams HgI 2 .KI at 25. 

(Mehu.: 

SOLUBILITY OF MERCURIC IODIDE IN OILS. 



(Anon, 1903, 1904.) 



Oil. 

Castor Oil 
Walnut " 
Linseed " 
Cod Liver " 


Gms. Hgl t 
per loo cc. 
Oil. 

1.90 
I .29 
1.23 

-S4S 



Oil. 



Peanut Oil 
Olive " 
Almond " 
Vaseline 



Gms. Hgl| 

per loo cc. 

OU. 

0.52 
0.45 

-39 
0.26 



Hg HYDRARGYRUM 



648 



SOLUBILITY OF MERCURIC IODIDE IN PYRIDINE. 

(Determinations from 50 to 98.5 made by saturating the solvent at con- 
stant temperatures are given by Mathews and Ritter (1917). Measurements of 
the points of solidification of various mixtures of the two components, covering 
the range from IO to 135, are given by Staronka (1910). 



t. 


Gms. Kg!, 
per loo Gms. Solid Phase. t. 


Gms. HI 2 
per loo Gms. Solid Phase. 




Sat. Sol. 


w 


Sat. Sol. 




-50 


1.93 HgI 2 . 2 C 5 H 6 N 90-. 08 


61.43 Hgl,. 


2C S H S N 


3 1 -5 


4.27 


" IOO 


65.7^ 




10 


10.28 


105 


68.89 * 




o.i 


14.85 


107 m. pt. 


72.09 ' 




+ 8.83 


18.42 


105 


75-67 




20.02 


24.40 


IOO 


79-73 * 




25-55 


27.90 


90 


84.16 




40.08 


37-^4 


87 Eutec. 


85.17 " 


+HgI 2 .C 6 H s N 


50.02 


43 ^S 


IOO 


86 ] 




60.07 


48.29 


120 


87.16 


" 


80.05 


57.60 


135 


88.78 


" 




SOLUBILITY 


OF MERCURIC IODIDE IN 


QUINOLINE. 








(Staronka, 1910.) 






r. 


Mols. HgI 2 
per loo Mob. 
Hgf*+C,H,N. 


Solid Phase. t. 


Mols. HgI 2 
per 100 Mols. 
HgI 2 +CH 7 N 


' Solid Phase. 


IOO 


4-7 


HgI 2 . 2 C 9 H 7 N l6o 


37-7 


Hgl^C^N 


iiS-5 


9.1 


I6 5 


41 .6 


" 


133-5 


13.2 


I6 5 


43 


" 


133 


23.1 


170 


48.8 


" 


145 


26.7 


HglfrCsW ^9-S 


49-5 


" 


153 


3*-4 


166.5 


54-4 


K 


100 gros. 


liquid Sulfur 


Dioxide dissolve 0.012 


gm. HgI 2 at 


. ( Jand 



TINO_ 
T1SO, 



and Ruppolt , 1937. ) 

Fusion-point data are given for the following mixtures. 

(Bergmann, 1921, 1922-4, 1926.) 
(Paic, 1930, 1933.) 
(OUvari, 1908. ) 
(JBergmann, 1926. ) 
(Woskresenskaja, 1929.) 
MERCURIC Ammonium IODIDE HgI ? .2NH 4 I .H ? 

100 gros. sat. sol. of Mercuric 'Ammonium Iodide in Water contain 
22.6 gms. Hg, 4.5 gms. NH 4 and 62.3 gms. I at 26; d of sat. sol. 3 
2.98. (Duboin, 1905. ) 
MERCURIC IODIDE Diamine (NH,),HgI. 

Data for the solubility of diamine mercuric iodide in aqueous ammonia solu- 
tions at 20 are given by Francois (1900). The solid is not stable in solutions 
containing less than 48 gms. NHs per liter. 

MERCOROUS IODATE Hg p (I0 3 )g. 

The Solubility Product of Mercurous lodate in Water at 25 is 
1.3 x io" 18 as guoted from Spencer, 1912, by Brodsky, 1929. 



649 HYDRARGYRUM Hg 

MERCURY NITRATE (ic) Hg(N0 3 ) 2 , (ous) Hg 2 (NO 3 ) 2 . 

TOO gms. anhydrous lanolin (m. pt. about 46) dissolve 1.15 gm. Hg(NO 3 )2 
at 45. (Klose, 1907.) 

100 cc. anhydrous hydrazine dissolve about 2 gms. Hg 2 (NO 3 ) 2 with precipita- 
tion of Hg at room temp. (Welsh and Broderson, 1915.) 

MERCUROUS NITRATES 

EQUILIBRIUM IN THE SYSTEM, MERCUROUS OXIDE, NITROGEN 
PENTOXIDE AMD WATER AT 25. 

(Denhan and Fife, 1933.) 

In the case of the normal salt, mixtures of the required amounts of 
HNO ? , H g O and finely ground mercurous nitrate were shaken in sealed 
bottles until equilibrium was reached. For the preparation of the 
basic salts cither mercurous nitrate was shaken with the necessary 
amount of water or mercurons oxide was shaken with NN0 3 . The mercury 
in the saturated solutions was determined by electrolysis and the 
nitrate by a modification of the Devarda method. 

d. of sac. Oms. per too gma. sat., sol. Solid d of sat. Oms. per 100 gms. sac. sol. Solid 
solution / HggTS A NJ3I "* Phase solution ' HggO N^ ""Phase 

1.039 3.03 i.oo A 1.557 31.00 12.10 <* D 

1.058 4.64 1.40 " 1-447 26.88 12.27 " 

1.082 6.55 2.30 " 1.396 22.30 12.87 " 

1.095 7-57 2.44 " L382 21.21 13.30 " N Q 

1.113 8.66 3.01 " 1-359 19.25 14.00 ""^BD 

1.117 9-12 3.22 M +B 1.366 19.63 14.53* a ^ 

1.139 10.46 3.61 B 1.455 22.97 15.84* " 

1.200 15.10 5-44 " 1.464 23.30 16.20* " 

1.275 18.42 6.60 " 1.563 27.65 17.20* " 

1.328 21.10 7-70 " 1.638 30.80 18.00* " 

1.366 23.53 3.22 " 1.781 34-88 19.35* " 

1.450 27.28 9.61 H 1.485 26.38 13.29* 0D 

1.502 29.31 10.43 " 4 C 1.442 24.22 13 'S 5 * " 

1.510 29.70 10.50 C 1.405 22.12 13.82" " 

1.527 30.18 10.75 " 1-365 19.84 13.87* " 

1.565 31.76 11.20 " 1-359 19.25 14.00 " 

1.608 33.00 11.79 "+D 1.426 20.66 17.70 " 

* = Metastable 

A = 2Hg 2 O.N 2 O s .H 2 0; R = S Hf? 8 3N 8 6 . 3 H 8 0; C = 4Hg 2 0. 3 N 2 5 .H 2 0; 

D = Hg 2 (N0 3 ) 2 .2H 2 which exists in an d and ayg form. 

MERCURIC Ethyl and Other NITRATES 

SOLUBILITY OF EACH SEPARATE LY > T WATKR AT 25. 

(Johns, Peterson and Hlxon, lj:50.) 

Gtot. Mola. Compound 
Compound ^nula pdp llter ML- aoU 

Ethyl Mercuric Nitrate C 2 H fi ttRN0 3 0.0239 

Butyl " " C 4 H 9 Hc[N0 3 0.003 

Benzyl " " C 6 K B CH 8 HgNO B 0.00263 

^Xylyl " " C fl H 4 CH a ) 8 H?N0 8 0.00057 

Henyl " " C e HHgN0 3 0.00236 



Eg HYDRARGYRUM 

NERCUROUS OXIDE Hg g O 



65 o 



The Solubility Product of Mercurous Oxide in tfater at 25* is 1.8 x 
io"* 4 as quoted from Burgarsky, 18971 by Brodsky, 1929. 



MERCURIC OXIDE HgO 



t*. 



SOLUBILITY IN WATER. 

(Schick, 1903.) 

Gms. per rooo cc. Solution. 



25 
100 



0.0518 yellow HgO 
0.410 yellow HgO 



0.0513 red HgO 
0.3 79 red HgO 



At 25^the mixtures were constantly agitated for 4 days or longer. At 100 
the solutions were boiled and stirred tor 5 hours. A longer period would prob- 
ably have caused better agreement between the red and yellow HgO. 
One liter H 2 dissolves 0.05 gm. HgO (red, large grains) at 25. (Hulett, 1901.) 
One liter HaO dissolves 0.15 gm. HgO (red, finest grains) at 25. 

Very careful determinations of the solubility of yellow and of red 
Mercuric Oxide in Water - both determined directly and by extrapolation 
from measurements in aqueous alkali solutions-gave the value 0.000225 
gm. mols. (= 0.0487 gtn. ) of red HgO per 1000 gms. HO and 0.000237 gm. 
mols. (= 0.0513 gms.) of yellow IfgO per looo'gms. H 2 0, at 25. (Garrett 
and Hirschler, 1938.) 

One liter sat. sol. of lig(OIi) 2 in H g O contain 0.000251 gm. mol. 
(= 0.0544. gm.) HgO at 25. (lierz and "Hiebenthal, 1928.) 



SOLUBILITY OP YELLOW AND OF RED MERCURIC OXIDE IN 
AQUEOUS SOLUTIONS OF NITRIC ACID AT 25. 

(Garrett and Howell, io?S9.) 



Results for Yellow Mercuric Oxide 



Mols. per 



da. Mols. per 



-Jggggy- H P A tOQO ffltf. HyO 

3 x tO 4 HgOxld"* HNOyXlo" 4 HgO X 10~ 4 



Results for Red HgO 

Ota. Mols. per 

. 1000 aga. HgO 

HNO X ID"* HgO X to" 4 ' 



0.5 


2. 43 


156 


58.5 


700 


312 


1.0 


2.98 


1.0 


2.57 


20O 


65.5 


703 


312 


2.0 


3.14 


2.0 


2.67 


200 


68.0 


722 


329 


3.0 


2.77 


l.0 


3-11 


300 


111.0 


743 


333 


5.0 


3-'8 


6.0 


3-35 


30O 


108.0 


76i 


3M9 


7.0 


3.56 


8.0 


3.80 


noo 


173.0 


78o 


362 


9-0 


4-02 


10.3 


4.15 


400 


169.0 


976 


449 


2O. 


6.32 


20.0 


6.08 


500 


217.0 


1170 


536 


30.0 


9.17 


40.0 


12.1 


585 


236.0 


1370 


638 


50.0 


14.2 


60.0 


18.3 


600 


253.0 


140O 


596 


70.0 


20.2 


80.0 


23.2 


634 


262.0 


1560 


718 


90.0 


27.9 


106.0 


30.0 


683. 


299.0 


1600 


662 


200.0 


64.2 



The above values for HN0 3 are those of the solutions as made up. The 
solutions were maintained in an atmosphere of nitrogen. Calculations 
of the acidity corrected for the amount of acid used to reetct with the 
oxide are given. 



65* 



HYDRARGYRUM Hg 



SOLUBILITY OF MERCURIC OXIDE IN AQUEOUS HYDROFLUORIC ACID AT 25. 

(Jaeger, 1901.) 



Normality 
of HF. 

O.I2 
O.24 

0-57 
I. II 
2.17 



Cms. Hg per 
9.6 cc. Sat. Sol. 

0.0242 
0-0475 
O.I2IO 
O.2247 
0.4976 



Gm. Atoms Hg 
per Liter. 

0.01258 

0.0247 

0.0629 

0.1168 
0.2586 



SOLUBILITY OP MERCURIC OXIDE IN AQUEOUS SALT SOLUTIONS AT 25. 

(Herz and Hlebenthal, 1928.) 

Results for aqueous: 
Potassium Chloride Lithium Chloride Sodium Chloride 



On. Equivalents per liter 
~"KC1 ^ HS"O~ ^ 



On. Equivalents per liter 
__ 



On. Equivalents per liter 



0.35 
0,70 
0.85 
1*49 
2.35 
3.13 



0.0008 
0.0011 

0.0013 
0.0023 
0.0038 
.0.0054 



0.35 
0.51 
0.74 
0.99 

2.15 
2.47 



HgO 

0.0008 
0.0011 
0.0014 
0.0020 
0.0053 
0.0061 



Neci 


HgO 


1.05 


0.0026 


1.55 


0.0036 


2.12 


0.0046 


3.13 


0.0074 


4.22 


0.0091 


5-45 


0.0158 



MERCURY OXIDE (ic) HgO. 

SOLUBILITY OF MERCURIC OXIDE IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE 

AT 25. ( Fuseya, 1920. ) 

The mixtures were rotated in sealed tubes for at least 4 days. Equilibrium 
was approached both from above and below. 

Mols. NaOH MllUmols. HgO 

per lller of sat. sol. per lilor of sat. sol. 

O.5O2 20.6 







Millimols. HgO 
per HUM* of sat. .sol. 



Mols. NnOII 
per liter of sat. sol. 

O . OOOO 

o . 0096 y-4 -6 r 0758 28 . 3 

o.o5o3 ^4-7 2.09 'to. 9 

0.0955 -24.9 

It is pointed out by -Garret t and Hirscliler, 1938* that through an 
obvious error the above solubilitjejof HgO are 100 times too high. 

SOLUBILITY OF YBLLO* AND OP RBD MERCURIC OXIDB IN 
AQUBOUS SOLUTIONS OP SODIUM HYDROXIDB AT 35. 

(Oarretc and Hlrschlar, 1936.) 

The determinations were made in an atmosphere of nitrogen. Equilibrium 
was approached both from under saturation and super saturation. The 
alkali was determined by titration, using methyl orange as indicator. The 
mercury was determined by a potentiometric method. 

Results for Yellow HgO Results for Red HgO 



Gta. Mols. per 
1000 018. HgO 


On. Mols. per 
1000 g>a. H g O 
'NaOH HgO"^ 

0.3467 0.000249 
0.5995 0.000255 
0.8515 0.000265 
1.512 0.000282 
2.562 0.000296 
3.405 0.000306 
4.460 0.000312 
5.952 0.000311 


On. Hole, ptr 
1000 ga. H g O 
-HSiOH Hgff^ 

0.00088 O.000225 
0*0050 0.000225 
0*0093 0.000226 
0.0187 0.000224 
0.1064 0.000227 
0.3398 O.000231 
0.4406 0.000242 
0.58l8 0.000246 


On. Mols. per 
1000 $aa. HgO 


' NaOH HgO x 

o.oooio 0.000234 
0.00082 0.000238 
0.0018 0.000232 

0.0040 0.000237 

o.oioo 0.000237 

0.0207 0.000237 
0.1015 0.000244 
0.2230 0.000241 


' NaOH HgO N 
0.7223 0.000251 

I. ooi 0.000262 

1.638 0.000272 
1.987 0.000276 
2.940 0.000294 
3.956 0.000297 
4.936 0.000298 



Eg HYDRARGYRUM 652 

SOLUBILITY OF YELLOW MBRCDRIC OXIDE IN AQUEOUS ALKALIES AND 
ALKALINE SALT SOLUTIONS AT 25. 

(Garrctt, and Hlrschltr, 1938.) 



OBJ. Mole, per 1000 gjoa. H g O 



OK. Hols, per 1000 gpia. H g O 





'Alfcall + Salt 


HgO N 'Altoll + 


dale 




Hgfl^ 






.1082 K 

.3038 


DH - 






.000240 
.000243 






.1328 NaOH 2 
. 1462 " i 


.400 KNO- 
.072 NaNO, 






.000384 
.000326 





.8175 


1 





.000253 





.1738 


" 2 


.637 " 





.000496 





.0689 L 


tOH 





.000239 





.1682 


11 6 


397 " 





.000753 





.2019 








. 000246 





1433 


" 


.5863Na.0, 


I 


.000301 





.4667 ' 





.000252 





.1380 


11 1 


.145 " 





.000347 





.1361 NaOH o.8iieC 


5 


.000291 





.1649 


II l 


.668 





.000370 





.1789 " 1-725 "' 





.000337 





.1454 


11 2 


.137 





.000390 



mqls. HgS = 0.0000125 'gm. at 18. 

(Weigel, 1906, 1907. See also Bruner and Zawadzki.) 



MERCURY SULFIDE HgS. 
One liter H 2 O dissolves 0.054 X 

(W 
MERCUROUS SULFATE Hgj>S0 4 

The Solubility Product of Mercurous Sulfate in Water at 25 is 4.7 x 
IS 7 as quoted from Bugarsky, 18971 by Brodsky, 1929. 

SOLUBILITY IN WATER, IN SULFURIC Aero AND IN POTASSIUM SULFATE AT 25 

(Drucker, 1901; Wright and Thomson, 1884-85; Wilsmore, 1900.) 
Solvent. Hg 2 S0 4 per Liter. 

Water 

Aq. H 2 S0 4 ( i . 96 gms.. per liter) 
Aq. H 2 SO 4 (4-90 gms. per liter) 
Aq. H 2 SO 4 ( 9.80 gms. per liter) 
Aq. K 2 S0 4 (34 87 gms. per liter) 

SOLUBILITY OF MERCUROUS SULFATE IN WATER AT DIFFERENT TEMPERATURES. 

(Barre, 1911.) 
Gms. per 100 Gms. Sat. Sol. 



Gm. Mol. 


Gms. 




11.71 to" 4 


0.,58 


(0.47 W. and T., 0.39 W.) 


8. 3 I " 


0.41 




8.78 " 


0.44 




8.04 " 


0.40 




9-OS " 


0-45 





16 -5 
33 
5 
75 
100 



- 
Hg 2 S0 4 . 

0.055 
0.060 
0.065 
0.074 
0.092 



-v 
H 2 S0 4 . 

0.008 
0.018 
0-037 
0.063 
0.071 



Solid Phase. 

Haso 



Bv 



. 

The mixtures were kept at constant temp, but not constantly agitated 
successive treatment of ^ a given amount of Hg 2 SO 4 with H.O, it is gradually 
converted to an almost insoluble basic salt, Hg 2 O.Hg 2 SO 4 .H 2 O. aauaiiy 

SOLUBILITY OF MERCUROUS SULFATE IN AQUEOUS POTASSIUM SULFATE 

SOLUTIONS. (Barre, 1911.) 

Results at 33. 

Gms. per 100 Gms. Sat. Sol. 



Results at 15*. 

Gms. per IPO Gms. Sat. Sol. 



^ 
H.SO, (free). 

0.0080 
5.70 0.0703 0.0093 
8.22 0.0912 0.0098 

I'll n'?T ' 
9.44, 0.1080 o.oiio 



' K 2 SO, Hg 2 SO, H 2 S0 4 (W. 

2.94 0.0677 0.0250 

5-68 0.1015 0.0350 

8.30 0.1364 0.0441 

I0 ' 7 - 1724 ' 438 

11.90 0.1902 0.0420 



Results at 75. 

Gms. per 100 Gms. Sat. Sol. 



K 2 SO, Hg 2 SO, H 2 S0 4 (free? 

3.10 0.1344 o 

5.75 0.2120 o 

8.50 0.2951 ' 

^' 20 -46io 0.2503 

17.30 0.6440 02225 



6 5 3 HYDRARGYRUM Hg 

SOLUBILITY op MBRCUROUS SULPATE IN AQUBOUS SOLUTIONS op SULPURIC ACID 

AT AND AT 28. 
(Craig, Vlnal and Vlnal, 1936.) 

Equilibrium was approached both from above and below. Mercury was de- 
termined electrolytically and the H-SO, in the electrolyzed solution was 
titrated. The acid equivalent to the Kg was subtracted from the total 
to obtain the H 2 S0 4 in the original solution. The results were plotted 
and the following average values obtained from the curve. 



Ota. Mols. H 2 S0 4 On. Hg per IQOcc aac. sol, at; &>. Mols. H g S0 4 On. Hg per IQOcc^sat. soL at; 
per lOOOcc solutlm' 6 * 26 ^ per lOOOcc solution'" ~" ^*" v 



0.001 
0.002 
0.004 
.0.006 
0.008 
0.010 
0.020 
0.040 
0.060 
0.080 






280 


0.0351 





0.0290 


0.0463 


0.0239 


0.0395 


0.0215 


0.0360 


0.0203 


0.0346 


0.0197 


0.0338 


0.0l82 


0.0318 


0.0178 


0.0317 


0.0178 


0.0327 


0.0l8o 


0.0337 



0.100 

0.200 

0.40 

60 

80 

00 

50 

00 

00 



4.00 





0.0183 
0.0198 


28 

0.0344 
0.0379 


0.0224 


0.0423 


0.0239 
0.0247 


0.0451 
0.0467 


0.0249 


0.0470 


0.024O 
0.0216 


0.0452 
0.0409 


0.0139 
0.0078 


0.0294 



closely with 



The above results calculated from 28 to 25 
the previous careful determinations of Hulett, 1904. 
MERCURY SULFATE (ic) HgSO*. 
EQUILIBRIUM IN THE SYSTEM, MERCURY OXIDE, SULFUR TRIOXIDE, WATER 

(Hoitsema, 1895.) 

Results expressed in molecules per sum of 100 molecules of the three com- 
ponents of the system. The mixtures were rotated for 3 hours or longer. 



Results at 25 



Results at 50. 



'H 2 0. S0 3 . 


HgO. 


oona jrnase. 


"TT Q i^Q 


Hgo: 


98 


5 


I. 


24 


0-33 


3 HgO.SO, 


9 8." 


9 


o 


.96 


o. 


I7 3 HgO.S0 8 


96. 


6 


2. 


49 


0.92 


" 


9 6 




3 


05 


o. 


93 


94-4 


3-93 i -&5 


93- 


2 


4 


.92 


I . 


90 


93- 


9 


4- 


24 


1-85} 


3HgO.SO; and 


92. 


8 


5 


.10 


2. 


09 


94.- 


4 


4- 


5 2 


2.12) 


3Hg0.2S0 3 .2H 2 


9 2 - 


8 


5 


.16 


2. 


06 


93- 


4 


4- 


65 


1.94 


3HgO.2SOs.2HaO 


92. 


5 


5 


-34 


2. 


12 


92-. 
92 


9* 
9 


4- 
5 


.81 
.11 


2.29 
1.98 


3 HgO.S0 3 
3Hg0.2S0 3 .2H 2 


92. 


2 


5 


57 


2. 


( 3 HgO.SO 3 and 

2O \ ,v cr . .j. 


92 


-3* 


5 


.20 


2-54 


3HgO!s0 3 


92. 


r 


5 


75 


2. 


1 1 3HgO.2SO s .2Hj 


92 


3 


5.58 


2.09 


3 HgO.2SOs.2H 2 


92 




5 


.80 


2. 


16 


92.1 
91.9 


5 
5 


97 


2.08 
2.90 


3HgO.S0 3 


91. 


,2* 


6 


.27 


2. 


. ( 3HgO.S0 3 and 
5 6 | HgO.SO a 


9* 
9 1 


9 
3 


6 
6 


54 


2.05 
2.13 


3 Hg0. 2 S0 3 .2H 2 


91. 


5 


6 


34 


2. 


1 9\ andHgO.SO a 


9i 


.2 


6 


-77 


2. 02 


HgO.S0 3 .H 2 


91. 


3* 


6 


37 


2. 


30 HgO.SO, 


9 1 


3 


6 


.90 


1. 80 


91.6 


6 


.69 


I , 


75 


9i 


3 


7 


.67 


I .OI 


" 


91, 


.1 


8.32 


O. 


57 


91 




7 


-84 


0.89 


HgO.S0 3 .H 2 and 


90 


5 


9 


.11 


O. 


4 


9 1 




8 


36 


0.69 


HgO.S0 3 


89.6 


10 


.2 


0, 


.23 


90 


5 


8 


95 


9-53 


" 


86 


7 


13 


.2 


O.O6 * 


89 


.2 


10 


.6 


O.22 


HgO.SO> 


3 1 


.6 


68 


4 


O 


.03 


75 


.8 


24 


.2 


trace 


* 














39 


.2 


60 


7 


trace 


" 


.U1-. AM, 













SO 



Hg HYDRARGYRUM 654 

SOLUBILITY op BASIC MBKCURIC SULPATR IN AQUEOUS SOLUTIONS 
op SULPURIC ACID AT 25-30. 

(Vosburgh and Lacfcey, 1930.) 

The mercury was determined by titration with standard thiocyanate 
solution. 

Oa. Mola. H S0 4 Q. MoU.^per liter 



per liter ' HgO SOj v 

0.0119/1- 0.00103 0.01228 

0.0954 0.0131 0.0998 

0.114.50 0.0203 0.1518 

100 gins, liquid Sulfur Dioxide dissolve o.oio gni. HgSO? at o. 
(Jander and Ruppolt, 1937.) 4 

Freezing-point data for mixtures of Hg g S0 4 + H g S0 4 are given by 
Kerfdall and Davidson, 1921. 
MERCURY SELENITE HgSeOa. 

SOLUBILITY IN AQUEOUS SODIUM SELENITE SOLUTIONS AT 25. 

(Rosenheim and Pritze, 1909.) 

Normality Gms. HgSe0 3 Normality Cms. HgSeOj 

of NaaSe0 3 per 100 Gms. Na^SeOa of per 100 Gms. 

Solution. Sat. Sol. Solution. Sat. Sol. 

0.0625 0.18 0.5 0.70 

0.125 0.32 I 1.39 

0.25 0.53 2 2.73 

HOLMIUM SULFATB Ho g (S0 4 ) 3 -8H 2 

100 gms. H 2 dissolve 8.181 gms. Ho g (S0 4 ) 3 .8H g O at 20 and 4.52 gms. at 
40. (Jackson and Reinacker, 1930.) 

IODIHE I 2 

SOLUBILITY op IODINB IN GASES AND THE VAPORS or SOLVENTS. 

Experimental determinations of the solubility of Iodine vapor in air 
are given by Baxter, 1907 and Baxter and Grose, 1915; in C0 8 and in H g 
by Braune and Strassmann, 1929; in air N~, , CH , CO and the vapors 
of CHC1 3 , CS 2 , CC1 4 , Hexane and Ethyl Ether, by Brflll and Ellerbrock, 
1934. 

SOLUBILITY OP IODINE IN WATER. 



The results of Sammet, 1905; Carter, 1925, 1928; Hartley, 1908; Lanza, 

1931* and Kracak, 1931, were plotted on cross section paper and the 
following values read from the average curve. 

Ctas. I per Otas. I per Q On. I per 

c liter sac. sol * liter sat. sol. c liter sat. sol. 

0.14 30 0.385 80 ,2.2$ 

10 0.20 40 0.52 90 3.15 

20 0.285 50 0.71 10O 4.45 

25 0.335 60 i.oo 106 5.60 



655 IODINE I 

Lanza found that supersaturation occurs easily, especially at the higher 
temperatures, and such solutions give up their iodine very slowly. 

By means of determinations made in sealed tubes by the synthetic method, 
Kracek found that above 112.3 two liquid layers are formed. The critical 
solution temperature, estimated to be above 300, could not be reached 
because of the extremely high vapor pressure developed by the system. The 
following points on the curve for the liquid layers were determined. 

Aqueous Layer Liquid Iodine Layer 

c Gma, I. per 100 gne. liquid laytr t 0s. I par 100 gms. liquid layer 

126.5 0.976 112.3 99.907* 

143. 2 1.422 155 99-712 

156.4 1.947 186 99.530 

175.9 3.082 >225 99'083 

188.4 4.125 

206.7 6.587 

SOLUBILITY OF IODINB IN AQUBOUS SOLUTIONS OF HYDROBROMIC ACID. 

(Lee and Lee, 1936.) 

Qm. Hols. HBr Qm. Mols. I 2 per liter sat. solution at: 

per liter sat. sol. 

0.05 
0.100 
0.588 
1.209 
1.851 
3.182 
SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF BARIUM IODIDE AT 25. 

(Pearce and Eversole, 1924.) 

Gm. mols. per 1000 gms. H a O Gm. mols. per 1000 gins. 11*0 

BaI 8 . I s . Iial a . I 8 . """ 

o.oooo 0.001829 0.16497 0.16872 

O.OOO686 O.OOUO44 0.3488O 0.39500 

o. 008120 0.004482 0.39633 0.45460 

0.006287 0.007674 0.07189 0.81690 

o. 031674 0.032199 0.87640 i.4<>74 

o. 047716 0.0484 i 3 1.1922 2.2880 

0.080477 0.079370 

SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF HYDROBROMIC ACID, 

HYDROCHLORIC ACID AND OF HYDRIODIC ACID. 

( OHveri-Mandala and Angeniea, 1920. } 

fn aq. HBr at 25. In aq. HG1 at 25.4. In aq. HI at 25.2. 

Gm. mols. per liter Gm. mols. per liter Gm. mols. per liter 

"H BrT"*"""^""*"^ 1,7^ ""HCl." 1 " 1 " J "'"" I,. ""* ~""m7~" ^~*~~l^ 

o.5oo 0.0081 o.5oo 0.00170 0.0604 0.029:) 

O.635 0.0096 1. 1*280 0.00256 0.0922 0.0459 

1.2433 o.o2o3 i.554o o. 00820 0.1209 0.0610 

1.8649 0.0828 1.8010 0.00878 0.2110 0.1117 

2.7978 o.o5i4 2.0589 o.oo43o 0.8120 o.i633 

0.7297 0.0750 2-553o o.oo5u 0.4280 0.2358 

2.8189 o. 00640 o.5ooo 0.8000 

3.855o 0.00780 o.635o 0.8950 

Results for the solubility of iodine in aq. H Cl solutions at 25, which do not 
agree with the above, are given by Ray and Sarkar, 1922. 



' 1 -O 
15 

0.00167 


26 
0.00221 


3150 
0.00281 


45 
0.00302 


0.00241 
0.00849 
0.01678 
0.02720 
0.0424! 


0.00319 
0.01O48 
0.02109 
0.03284 
0.05192 


0.00400 
0.01348 
O.O2690 
0.04165 
0.06478 


0.00533 
O.01766 
0.03511 
0.04878 
0.08354 



I IODINE 



656 



SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF NITRIC ACID. 



Results at 10. 



Wt. per cent 

II.So 
23.88 
32.35 
40.82 

49-5? 

55.82 

64.3o 
70.00 



Cm. mols. I, 
per liter. 

o . 000969 

0.001035 
0.001020 
0.000985 

o . 000957 
o . 000962 

O.OOIO8 
0.00178 



( Carter, 1925. ) 

Results at 23 tt . 

Wi. per cent 
HNO,. 



10.91 

33*.62 
42.28 

5-2.77 
63. 81 
69.65 
72.60 



Gm. mols. I, 
per liter. 

0.00160 
0.00179 
0.00186 

o.ooi85 
0.00189 
O.OO236 
o.ooSig 
o . 0039/1 



Results 

Wt. per cent 
UNO,. 

3.3i 

6.5o 
i5.5o 
28.72 
42.63 
43.i3 
58.37 



at 35o. 

Gm. mols. L 
per liter. 

0.00187 
O . OO2O4 

0.00233 
o . 00260 
0.0027.5 
0.00278 
o.oo368 



SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF ACIDS. 



Aqueous Acid. 

o.ooinHCl 
o.iowHNOa 



Mols. I per Liter 
Sat. Sol. 



Cms. I per Liter 
Sat. Sol. 



Authority. 

(Bray and MacKay, 1910.) 
(Sammet, 1905.) 



0.001332 0.338 

0.001340 0.340 

0.001342 0.341 

SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF SULF.URIC ACID AT 2o 

(Carter, 1925.) 



Wl. per cent 
II S S0 4 . 



22 . 72 

33.25 

40.42 



Gm. mols. I, 
per liter. 

0.00102 
O.OOO82 

0.0006 I 5 

O.OOO545 



olor 


Wt. per cenl Gm. mols. I s 


Color 


>lutlon. 


HjSO,. per liter. 


of solution. 


rown 


59.53 o.ooo38o 


Pi nkish-h brown 





72.04 0.000270 


Pink 





87.37 0.000200 






+ Pinkish 



SOLUBILITY OP IODINE IN AQUEOUS SOLUTIONS OP HYDEIODIC ACID AT 25. 

(Carter and Hosfclns, 1929.) 



On. Mols. pr 1000 gn. Mola. H g O 

_ ftC- 



OB. Mola. pr 1000 ga. Mola. H g O 



0.2117 
0.5284 
0.8810 



0.1326 
0.2956 
0.4715 



1.321 
1.763 
4.964 



0.7908 
0.9228 
2.784 



SOLUBILITY OF IODINE IN AQUEOUS MERCURIC CHLORIDE AND IN AQUEOUS 
CADMIUM IODIDE SOLUTIONS AT 25. 

In Aq. Cdl2- 
(Van Name and Brown, 1917.) 



In Aq. HgCl 2 . 

erz and Paul, 1914.) 



(Herz and 



Mfllitnols per Liter. 


Cms. per Liter. 


Gms. per Liter. 


Hg. 
o 

94-44 
124.42 
I9S-42 
334-00 


i~34 
12.94 
14.60 
18.06 
25.43 


HgCl,. 
o 

25.64 
33-78 
54.29 
90.84 


I. ' 
0.340 

3.285 
3.706 
4.583 
6.454 


' Cdl,. 
3-66 
45.78 
91-56 
183.12 


I. 

2.072 
9.056 
H.386 
14 . 040 



657 



IODINE I 



SOLUBILITY OP IODINE IN AQUEOUS SOLUTIONS op CHLORIDES AT 25. 
(Carter and Hosklns, 1929.) 

In Aqueous Solutions of: 
Hydrochloric Acid Potassium Chloride Magnesium Chloride Barium Chloride 



Gm. Mols. per 1000 
gn. Mols. H 



8.48 
17.9 
25. 
31- 
65. 
79- 
109. 



0.0431 

0.0655 

0.0793 

0.0951 

0.170 

0.197 

0.252 



141.0 0.299 



Om. Mols. per 1000 
gnu Mols. HgO 


KC1 


l z 


6.15 


0.0349 


12.3 


0.0438 


24.6 


0.0589 


36.3 


0.0711 


48.2 


0.0822 


60.6 


0.0905 


73-9 


0.0975 


86.8 


0.1003 



On. Mols. 


per 1000 


gn. Mols. H g O 


'1/2 MC1 2 ' 


~^~" 


8.48 


0.0394 


13-0 


0.0465 


26.3 


0.0634 


53-5 


0.0741 


67.5 


O.O750 


96.1 


0.0732 


125.9 


0.0636 


141.3 


0.0573 



Qm. Mola. per 1000 
gm. Mola. H0 



3.67 

4.89 

12. 1 
24.0 

35-6 
46.9 
57.8 
68.6 



0.0305 
0.0318 
0.0426 
0.0538 
0.0610 
0.0660 
0.0676 
0.0671 



The authos also give results for the solubility of iodine at 25 in 



aqueous solutions of NaBr + Na 2 S0 4 , Nal 



NaN0 3 and Nal 



SOLUBILITY OP IODINE IN AQUEOUS SOLUTIONS OF CHLORIDES AT 25 

(Herz and Hlebenttal, 1939.) 



In aqueous solutions of: 
Lithium Chloride 

Om. Mols. per liter 
sac. solution 



Sodium Chloride 

3. Mols. per liter 
sac. solution 



Potassium Chloride 

On. Mols. per liter 
sat. solution 



0.46 
0.96 
1.98 
3-90 
6.43 
12.08 



O.00379 
0.00503 
0.00679 
O.00746 
0.00596 
0.00127 



Magnesium Chloride 



Om. Mols. per liter 
sat. solution 


' 1/2 HgClg 


' ^ 


0.39 


0.00339 


0.59 


O.OO419 


1.49 


0.00620 


3.00 


0.00764 


4.55 


0.00718 


9-72 


0.00148 



0.20 


0.00274 


0.20 


0.00276 


0.44 


0.00344 


0.34 


0.00292 


1.23 


0.00511 


0.64 


0.00389 


2.39 


0.00612 


1.93 


0.00670 


3.45- 


0.00613 


2.75 


0.00800 


5-34 


0.00534 


4.85 


0.00756 



Strontium Chloride 



dm. Mola 


. per liter 


sat. 


solution 


1/2 SrCl 


* ^ 


0.46 
0.86 


0.00371 
0.004.68 


1.46 
2.37 
4.<u 
6.16 


0.00571 
0.00665 
0.00637 
0.00489 



Barium Chloride 



Qm. Mols. per liter 
sat. solution 


1/2 BaCl p 


'E 


0.23 

0.52 
0.83 


0.00278 
0.00388 
0.00453 


1.59 
2.70 
3.35 


0.00571 
0.00675 
0.00675 



I IODINE 658 

IODINE I 2 

SOLUBILITY OF IODINK IN SOLUTIONS OP VARIOUS SALTS IN WATER AND IN 
SOLUTIONS OP THE SAME SALTS IN 0.025 NORMAL POTASSIUM IODIDB AT 25. 

(v. Klsa and uraancay, 1931.) 


On. Mola. Salt 


On. Mola. I g ^ 


per liter in: 


Gto. Mols. Salt 


Gta. Mola. I per liter in: 


per liter 


^ H ^ 


0.6281 KI x 


per liter 


M J> 


o.osen KI 




Solution 


Solution 




Solution 


Solution 


0.0 


0.001332 


0.01362 


0.5 NaNO, 


0.001238 


0.01280 


0.5 KCI 


0.003306 


0.01342 


1.5 " 


0.001048 


0.01146 


1.0 " 


0.002821 


0.01308 


3-0 


0.000780 


0.00798 


1.5 


0.003315 


0.01271 


S.o " 


0.000573 


0.00567 


2.0 " 


0.003753 


0.01250 


7.5 


0.000369 


0.00370 


3.0 " 


0.004476 


0.01231 


0.5 LiNO, 


0.001270 


0.01292 


4.0 " 


0.004890 


0.01219 


1.5 " 


0.001187 


0.01202 


0.5 NaCl 


0.002083 


0.01306 


3.5 


0.001033 


0.01045 


1.5 " 


0.002960 


0.01196 


5.5 


0.000856 


0.00886 


3.0 


0.003320 


0.00987 


8.7 


0.000564 


0.00586 


5.0 


0.002942 


0.00707 


0.5 K p S0 4 


0.001190 


0.01246 


0.5 Lid 


0.002330 


0,01351 


1.0 " 


0.001034 


0.01126 


1.5 " 


0.003246 


0.01270 


1.37 " 


O.OOO909 


0.01052 


3-5 " 


0.003876 


0.00971 


0.25 Na g S0 4 


O.OO1210 


0.01283 


6.0 


0.003275 


0.00655 


0.75 * 


0.001052 


0.01139 


9.0 H 


0.002012 


0.00349 


2.0 


0.000705 


0.00837 


13-0 " 


O.OO0301 


0.00136 


3.5 


o . 000440 


0.00526 


0.6714 C a dg 


O.O02505 


0.01338 


0.5 Li SO 


0.001127 


0.01224 


1 1 .676 " 


0.003675 


0.01265 


15 


O.OO0798 


0.01015 


3-35 


0.004382 


0.01080 


3.0 " 


O.OO0474 


0.00692 


5-025 " 


0.003811 


0.00869 


5-0 


0.000238 


O.O0386 


6.714 " 


0.003136 


0.00671 


0.6855 Mg(N0 3 ) g 


0.001230 


0.1303 


0.6882 MtjCl,, 


0.002492 


0.01314 


1.714 " 


0.001053 


0.01193 


1.72 " 


0.003595 


0.01240 


3-427 " 


0.000891 


0.01045 


3-441 " 


0.003959 


0.01023 


5-135 " 


0.0006714. 


0.00874 


5.162 " 


0.003752 


0.00774 


6.855 " 


0.000550 


0.00717 


6.882 " 


0.002999 


0.00565 


0.5 MgSO 


0.001174 


0.01239 


0.5 BaCl g 


0.002226 


0.01286 


3.0 


0.000600 


0.00742 


1.5 " 


0.003035 


0.00941 


5.0 


0.000351 


0.00396 


3-0 


O.OQ3550 


0.00665 


0.5264 Ca(N0 3 ) g 


0.001229 


0.01314 


0.5 KNO S 


0.001257 


0.01305 


1.316 " 


0.001097 


0.01234 


1.0 " 


0.00ll6l 


0.01277 


2.632 " 


0.000910 


0.01104 


2.0 


O.001041 


0.01215 


3.948 " 


0.000736 


0.00967 


3-0 " 


0.000902 


0.01178 


5.264 " 


0.00o6l5 


0.00854 








0.25 Ba(N0 3 )_ 


0.001300 


0.01286 








o . 50 " 


0.001243 


1.01249 



SOLUBILITY OP IODINE IN AQUKOITS SOLUTIONS OP MIXTURES OP SALTS AT 25. 

(LaMer and Lewlnsohn, 1934.) 



Gta. Mola. Salts per liter 



0.0 (= H 2 at/a// 5.0) 

2.0 KNCL * o. 0025^1 
1.65 KCI * o.io KI 



0.001321 
0.002138 
0.004421 



Results are also given for a number of other mixtures of salts. 



659 IODINE I 

SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF POTASSIUM IODIDE AT 25. 

(Linhart, 1918.) 



Mols. KI per 1000 gms. H 2 o.4i36 

Mols. J 2 " o.23i3 



o.5g54 
0.3538 



o.8o65 

0.5176 0.7079 

SOLUBILITY OF IODINE IN VERY DILUTE AQUEOUS SOLUTIONS OF POTASSIUM 

IODIDE. . 

(Determinations made with very great care.) 

Results at o. Results at 25. Results at 25. 

(Jones and Hartman, 1915.) (Bray and MacKay, 1910.) (Noycs and Seidenstricker, 1898.) 



Normality 
of Aq. 


* o 


Gms. I per 
zoo Gms. 


Normality 
of Aq. 


Millirnols la 
per Liter 


Normality 
of Aq. 


Millirnols I 2 
per Liter 


KI Sol. 


Sat. Sol. 


Sat. Sol. 


KI Sol. 


Sat. Sol. 


KI Sol. 


Sat. Sol. 


0.000992 


I.OOO2 


0.0282 





1-333 





1.342 


O.OO2OO 


1.0004 


0.0409 


0.001 


1.788 


0.00083 


1.814 


0.00500 


I. 0010 


0.0760 


O.OO2 


2.266 


0.00166 


2-235 


0.01000 


1.0020 


0.1356 


0.005 


3.728 


0.00664 


4,667 


0.01988 


1.0044 


0-2533 


O.OIO 


6.185 


0.01329 


8.003 


0.0500 


1.0109 


0.609 


O.O2O 


11.13 


0.02657 


14-68 


0.09993 


1.0219 


1.199 


0.050 


25.77 


0-05315 


28.03 








0.100 


51-35 


0.1063 


55-28 



SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF POTASSIUM IODIDE AT 
25 AND VICE VERSA. 

(Parsons and Whittemore, 1911.) 
(Time of rotation 6 mos. or longer. Duplicate determinations at different lengths of time, were made.) 



Sp. Gr. 
Sat. Sol. 


Gms. per 100 Gms. _ 
Sat.^Sol. | 


>olid Sp. Gr. 
base. Sat. Sol. 


Gms. per 
Sat. 


loo Gms. 
Sol. 


Solid 
Phase. 


'KI 


I 


KI 


I 


1-349 


16.03 


1 8 . 49 Iodine 3 . 246 


27.92 


66.45 


KI 


1.516 


19.70 


26.16 


3-232 


29.71 


62.81 





1.769 


22.88 


36.06 


2.665 


35-80 


49-61 


" 


1.910 


23-55 


40.52 


2-539 


38.09 


44.58 


" 


2.403 


24.78 


53-6o 


2.216 


44.82 


31.01 


u 


2.904 


25 


63.12 


2.066 


49.04 


23.08 


tt 


3-082 


25.18 


66.04 


1.888 


54-41 


11.63 


" 


3.3l6 


26 


68.09 +KI 1-733 


60.39 


o 





Additional data for this system are given by Bruner, 1898; Hamberger, 1906; 
and Lami, 1908. 

Data for the solubility of iodine in aq. 40% ethyl alcohol and aq. 60% ethyl 
alcohol solutions of potassium iodide at 25, are given by Parsons and Corliss, 
IQIO. The solid phases were identified in each case and it was demonstrated 
tnat 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 iodida 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 
I 2 /KI was found to be i or more in all cases. 

A review of the evidence for and against the existance of potassium 
tri iodide is given by Bancroft, Scherer and Gould, 1931. The authors 
verified one of the results (analysis No. 8) of Parsons and Wiittemore, 
1911, of which there appeared some doubt. This was done by adding an 
excess of either iodine, potassium iodide or so-called potassium tri 
iodide to a synthetically prepared solution corresponding to the quad- 
ruple point of the system. No change in the composition of the solution 
occurred. From this and other evidence it was concluded that potassium 
tri iodide does not exist at 25. 

For additional results upon the system I + KI see under Potassium 
Iodide. 



I IODINE 



660 



SOLUBILITY OF IODINB IN AQUEOUS SOLUTIONS OF POTASSIUM IODIDE AT 25. 

(Relchsteln, Ewentow and Kasarnowsfcy, 1933.) 



df of 
sat. sol. 



On. Hols. KI 
per liter 



Ratio I 

KI 



d 5 of am. Mols. KI 
sat. sol. per liter 



008 
025 
055 
095 
255 
335 
390 
508 
512 
l .652 
1.760 



0.055 


0.96 


1.776 


2.870 


0.136 


1.00 


1.889 


3.281 


0.273 


1.08 


1.900 


3.315 


0.5<H 


1.15 


2.006 


3.647 


1.052 


1.39 


2.090 


4.024 


1.330 


1.50 


2.200 


4.376 


1-551 


1.59 


2.289 


4-710 


1.985 


1.74 


2-357 


5.030 


2.001 


1.75 


2.390 


5.160 


2.448 


1.91 


2.S04 


5.630 


2.809 


2.07 


2.640 


6.259 



2.09 
2.23 
2.25 



2.45 

2.56 

2.69 

2.82 
2.83 
2.98 
3.17 



The mixtures were rotated constantly for 200 hours. The saturated 
solutions were analyzed by diluting an unweighed portion of the filtered 
solution with water and distilling the free iodine into KI solution. 
This was titrated with thio sulfate and the fixed iodine remaining in the 
distilling flask titrated with silver nitrate according to Volhard. The 
densities of the saturated solutions were measured in a i.scc pycnometer. 
The authors also give results in the form of a diagram showing the effect 
of additions of sugar upon the ratio of T/KI at different KI concentra- 
tions. The presence of sugar increases the solubility of I at low con- 
centrations of KI and diminishes it at high concentrations. 



EQUILIBRIUM IN THE SYSTEM IODINE, POTASSIUM IOOIDE AND 
WATER IN THE REGION OF Low WATER CONCENTRATION AT 25. 

(Grace, 1931.) 

The mixtures were initially heated to about 50 and then rotated at 
25 for one month. Both the sat. solution and moist solid phases were 
analyzed. The diagram and the analyses confirm the existance of the two 



polyiodides KI 3 .H, 

Ons. per ioo Rjns x sat. 


p O and KI ? .H ? 0. 
solution Solid 


' T ? 


KI 


H 2 


v Phase 


57.83 


32.18 


9.96 


KI 


61.97 


30.25 


7.8 3 


+KI 3 .H 2 


63.40 


29.09 


7.45 


KI . H 


63.88 


28.92 


7.16 


M 


64.85 


28.36 


6.87 


II 


66.10 


27.26 


6.59 


* KI 7 



Qms. per 


100 gws^sat. 


solution 


Solid 


l ? 


KI 


H^ 


Phase 


66.65 


27.04 


6.38 


KI ? .H E 


67.34 


26.52 


6.20 


ii 


68.02 


26.00 


6.00 


" + I 


65.98 


25.08 





I 



The author also gives several experiments upon equilibrium in the 
non aqueous solvents, tetra chlor ethane and benzene. 



661 

SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF POTASSIUM BROMIDE 
AND OF SODIUM BROMIDE AT 25. 

(Bell and Buckley, 1912.) 
In Aq. KBr Solutions. In Aq. NaBr Solutions. 



IODINE I 



Gms. KBr 


Gm. Atoms I 


per Liter. 


per Liter. 


60.6 


0.0176 


106.9 


0.0278 


175-9 


0.0415 


22Q.8 


0.0532 


281.9 


0.0628 


330-6 


0.0717 


377-1 


0.0797 


411 


0.0864 


461.7 


0.0948 


509.8 


0.1006 


567. 9 sat. 


o . 1094 



Gms. NaBr 


Gm. Atoms I 


per Liter. 


per Liter. 


96.4 


0.0266 


187.7 


0.0425 


271.8 


0.0538 


357-4 


0.0598 


422.21 


0.0638 


499.1 


o . 0648 


569.9 


0.0644 


632 


O.O622 


679.7 


0.0595 


750.5 


0-055I 



756.1 sat. 
SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AND OF 

SODIUM NITRATE. (Carter, 1925.) 
Results for Sodium Chloride Results for Sodium Nitrate 



Wt. 

per cent 



NaCl. 

4.52 

7-43 

14.14 

20. 3l 

23.t5 
25.95 



at 25. 

Gm. mo Is. I, 

per 1000 gm. mols. 

11,0. 



a i 28K 



o.o44o3 
0.05295 
0.06289 
o . o63 i i 
o.o6io5 
0.05790 



Wt. 

per cent 
NaNO a . 

5.89 
1 1. 10 
I5.3I 
25.67 
29.75 
35.43 

39.83 



Cm. mols. I, 

per 1000 gm. mols. 

H 8 0. 



at 


35". 


Wt. 


Gm. mo Is. I, 


per cent 


per 1000 gm. mols. 


NaNO v 


H,0. 


1.98 


0.0827 


3.48 


O.O3'2O 


6.85 


0.0802 


15.89 


0.026tf 


29.06 


O . O2O T 


40.17 


0.0143 


5o. i 


O.OIOO 



0.0222 
O.O202 

o.oi85 
0.0145 

0.0125 

0.0108 
o . 009 i i 
0.00753 
SOLUBILITY OF IODINE IN AQUEOUS SODIUM IODIDE SOLUTIONS. 

(Gill, 1913-14.) 

Aqueous Nal solutions were prepared by dissolving the stated amounts of the 
salt in water and diluting to 100 cc. An excess of iodine was added to each of 
these solutions, the mixtures heated to 60 and shaken for several minutes. 
They were then allowed to cool in a thermostat at 25 for four hours. The 
dissolved iodine in weighed amounts of the saturated solutions was titrated with 
thiosulfate. The densities of the Aq. Nal mixtures, and also of the solutions 
after saturation with iodine were determined. 

Gms. Nal <* of <* 2B of Aq. Nal 

per 100 cc. Aq. Nal after Saturation 

Aq. Solution. Solution. with I. 

5 1.0369 1.0698 



Gms. 1 Dissolved 
5 per too Gm 
f the Sat. Sol. 

4-99 



at 25 per too Gms. 
oft! ~ " ' 



IO 

IS 
2O 



1.0720 
I .1072 
I.I458 



I.I4I5 
I.2I62 
I . 2998 



9.96 

H-93 

20.02 



Determinations at other temperatures were made in an apparatus which per- 
mitted constant stirring of the solutions at the several temperatures. Results, 
interpolated from the original, are as follows: 



Gms. I Dissolved per 100 Gms. 
Sat. Solution in Aq. Nal of: 



l> . 


10 Gms. per 


20 Gms. per 




100 CC. 


IOO CC. 


ro 


8. 9 


17.6 


15 


9-3 


18.3 


20 


9.6 


19 


25 


IO 


19.4 



Gms. I Dissolved per 100 Gms. 
Sat. Solution in Aq. Nal of: 





10 Gms. per 

IOOCC. 


20 Gms. per 

IOOCC. 


30 
40 


10.3 

10.9 


20.5 
22 


50 
60 


11.7 

12.6 


23-4 
24.9 



I IODINE 662 

SOLUBILITY OP IODINB IN AQUEOUS SODIUM IODIDB ALONB 

AKD CONTAINING SODIUM SULPATB AT 35. 

(Carter, 1928.) 



Results for: 

AIJ. Nal Solutions 



Nal 



0.0 

0.00039^ 

0.000784 

0.001959 
0.003918 
0.007838 
0.01959 



0.001324 
0.001494 
0.001676 
0.002260 
0.003199 
0.005126 
0.01096 



Aq.. Nal 
On. Mols. par J.OOO gaa. H g 

1.698 



Na g S0 4 Solutions 

a. H g O dm. Mols. I 

,80.. ^ par 1000 ] 



0.000251 
0.000655 
0.001431 
0.003271 
0.006531 
0.01274 
0.02619 
0.05253 
SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF MONO SODIUM PHOSPHATE 

AND OF SODIUM SuLFATE. (Carter, 1925.) 



0.000413 
0.000497 
0.000666 
0.001048 
0.001738 
0.003063 
0.006031 
0.01190 



Results for NaH,(P0 4 ) 2 
at 25. 



Results for Na 2 SO A 
at 23. at 35 





Gm. mols. I 4 




Gm. mo Is \ 




Gm. mols. I. 


Wt. per cent 


per jooo gins. 


Wt. por cenl 


per 1000 gms. 


Wt. per cent 


per 1000 gin* 


NaIl s (PO,) s . 


mols. FI 4 0. 


Na a S0 4 . 


mols. 11,0. 


Na 8 SO,. 


mols. ir.,,0. 


7-53 


O.OI94 


5.66 


O.OI73 


i.o5 


o.o3i8 


14.40 


0.0161 


8.64 


0.0144 


4-93 


0. 0/25 -A 


20.64 


0.0135 


1 6 . 2,4 


o.oo855 




O.O2O2 


26.4 


O.OIII 


19.66 


0.006 56 


14-79 


0.0133 


3i.66 


o . 00893 






21.10 


0.008 3g 


4r.o6 


o.oo4 3 






25 . 3 1 


o.oo585 


45.ot(> 


o 0018 






33.io 


0.00^58 



SOLUBILITY OF IODINE IN AQUEOUS SALT SOLUTIONS AT 25 

(McLauchlan, 1903.) 



Salt 

NaaSOi 



NaN0 3 
KN0 3 



Gms. Salt 
per Liter. 


Gms. Dissolved 
I per Liter. 


29.77 


0.160 


43-5 


0.238 


33 


0.246 


35 


0.257 


IOI.2 


0.266 


80 


0.375 


58-5 


0.575 


73-6 


0.658 



[Salt. 


Cms. Salt, 
per Liter. 


Gms. Dissolved 
I per Liter. 


NH4C1 


53-4 


o-735 


NaBr 


103 


3-29 


KBr 


119 


3.801 


NHiBr 


98 


4.003 


NHiCjHA 


77.1 


0.440 


(NH4) 2 C 2 4 


86.9 


0.980 


HaBOs 


SS-8 


0.300 



NaCl 
KC1 

SOLUBILITY OF IODINE IN AQUEOUS ETHYL AND NORMAL PROPYL ALCOHOL 
SOLUTIONS AT 15. 

(Bruner, 1898.) 



In Aq. Ethyl Alcohol. 



In Aq. (n.) Propyl Alcohol. 



V H*dl 


Gms. I per 


Vol. % 


Gms. I per 


Vol. % 


Gms. I per 


Vol. % 


Gms. I per 




IOOCC. 


CH 5 OH 


IOOCC. 


CjHjOH 


IOOCC. 


CgH^OH 


TOO CC. 


inSolvent. 


Solution. 


in Solvent. 


Solution. 


in Solvent. 


Solution. 


in Solvent. 


Solution. 


10 


0.05 


60 


I.I4 


10 


0.05 


60 


2.71 


20 


0.06 


70 


2-33 


20 


O.II 


70 


4.IO 


30 


O.IO 


80 


4.20 


30 


0.40 


80 


6.05 


40 


O.26 


90 


7-47 


40 


0.94 


90 


9.17 


50 


0.88 


IOO 


15-67 


50 


1.64 


IOO 


14-93 



663 IODINE 

SOLUBILITY OF IODINE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL AT 15., 
(Schoorl and Regenbogen, 1919.) 

Due to the ready formation of HI, accurate determinations of the solubility 
of iodine in aqueous alcohol can be made best by diluting a solution of iodine in 
absolute alcohol with water, and determining immediately the C 2 H 5 OH and iodine 
content of the resulting solution. At concentrations of alcohol less than 18 per 
cent the addition of water does not precipitate iodine from its saturated solution. 
The maximum precipitation of iodine occurs when just enough water is added to 
bring the alcohol concentration to 18 per cent. 

The determiriations were plotted and the following values read from the curve. 



Wt. per cent Gins. 1 \Vt. per UK) Cms. I Wt. per 100 Gins. I 
C 8 H 8 OH per UH) gins. C 2 H S OU per 100 gms. C.jir 6 OII per 100 gins. 


In aq.-alc. solvent. solvent. 


In aq.-ale. solvent. solvent. in nq.-ale. solvent. solvent. 


. O . O7.5 


35.o o.35 


70.0 4 


.3 


5.o o.o33 


4o.o o.55 


75.0 5 


.6 


10. 0,045 


45.0 0.80 


80.0 7 


.2 


i 5 . o o . oG 


5o.o i. 20 


85.o 9 


.0 


20. o 0.08 


55.o 1.70 


90 . o ii 


.4 


25. O.I I 


60 . o 2 . 3o 


95.0 14 


.8 


3o.o 0.20 


65.o 3.20 


IOO.O 20 


.0 


SOLUBILITY OF IODINE IN AQUEOUS ETHYL ALCOHOL AND IN 


AQUEOUS ACETIC 






ACID SOLUTIONS AT 25. 








(McLauchlan, 1903.) 






In Aq. C 2 H 6 OH 


Solutions. In Aq. CHaCOOH 


Solutions. 




Cms. QHsOH 
per 100 Cms. 
Solvent. 


pins. I per Gins. CHsCOOH 
100 cc. Sat. per 100 Gins. 
Solution. Solvent. 


Gins. I pec 
zoo cc. Sat. 
Solution. 







0.034 o 


0.034 




4-55 


0.039 20 


0.076 




28.48 


0.172 39.5 


0.173 




44.41 


0.955 61.1 


0.510 




72-51 


6.698 80.7 


1.363 




IOO 


24.548 loo 


3.162 





Since McLauchlan f s value for the solubility of iodine in water was 
apparantly too low, the figure 0.0311 gin. per loocc was substituted and 
used as a basis for calculating the remaining results for the solubility 
of iodine in aqueous alcohol and acetic acid. 

SOLUBILITY OF IODINE IK ETHYL ALCOHOL CONTAINING 
ONLY SMALL AMOUNTS o? WATIR. 

(Deleplne and Arquat, 1928.) 

Wt. Percent Ckaa. I par We. Percent Gtea. I par 

t o Vs * 1 in l **** "* C * C W H in 10 0Ba * 8ftt ' 

Solvimt Solution Solvent Solution 

IS 8$ 6.50 24.5 85 7.97 

" 90 8.SO " 90 10.2 

" 95 12.5 " 95 14-8 

" 99.8 18.7 " 99-8 21.0 

Several determinations of the reciprocal solubility of Iodine, Ethyl 
Ether and Water at 20 are given by Nesteroro and Petine, 1931. 

100 gms. Glycerol of d = 1.2326 ( z 86^5%) dissolve 0.47 gm. I at 30*. 
" " " " d = 1.26^5 <= 98.5%) " 0.67 " " " " 

11 (Holm, 1921-1922.) 

100 gms. Glycerol of d ls = 1.256 dissolve 2.0 gm. I at 15-16. 

(Ossendowaki, 1907.) 



IODINE 664 

SOLUBILITY OF IODINE IN AQUEOUS GLYCEROL SOLUTIONS AT 25. 

(Herz and Knoch, 1905.) 

Density of glycerine at 25/4 - 1.2555; impurities about 1.5%. 

Wt.% Glycerine Millimols I Grams I per Density of 

in Solvent, per too cc. Solution. 100 cc. Solution. Solutions at 2s/4. 

o 0.24 0.0304 0-9979 

7.15 0.27 0-0342 1.0198 

20-44 -38 0.0482 1.0471 

3 1 -55 -49 0.0621 1-0750 

40.95 0.69 0-0875 1-0995 

48.7 1.07 0.135 1.1207 

69.2 2.20 0.278 I-I765 

ioo. o 9.70 1.223 1.2646 
EQUILIBRIUM IN THI SYSTIM IODINI, PYRIDIN* AND WAT* a AT 18. 

(Chlttltt, 1934.) 

The solubility of iodine in pyridine was found to be about 450 gms. I 
per looocc of sat. solution at 18 . Prom such a solution upon evapora- 
tion, clear yellow needles separate, but within 2-5 minutes they begin to 
decompose with liberation of iodine. 

In the case of the mixtures of iodine, pyridine and water they were 
agitated about 15 minutes and then filtered through a porus glass disc. 
The clear filtrate and several samples of the mixture of solid and solu- 
tion were analyzed. The results when plotted indicate the formation to 
two molecular compounds. 

OM. pr 100 0M. *at. solution Solid 

PhMt 

I 2 (C 5 iI 8 N) g .29(?)H E 

" 

" 
I e (C B H B N).6H,0 



DISTRIBUTION OF IODINE BETWEEN WATER AND BROMOFORM, WATER AND CAR- 
BON BISULFIDE, AND WATER AND CARBON TETRACHLORIDE AT 25. 

(Jakowkin, 1895.) 

The original results were plotted on cross-section paper and the following table made from the curves. 
Jakowkin points out that the results of Berthelot and Jungfleisch, 1872, are incorrect on account of the 
presence of HI. 

Cms. I per Liter Cms. I per Liter of: 

of H S Layer 
in Each Case. 

O.OS 
O.IO 
0.15 
0.20 
0.25 

A theoretical discussion of the results of Jakowkin is given by Schtikarew (1901). 



3-6 


47.5 


48.9 


1.0 


33-9 


6 5 .i 


1*5 


24 >1 


74*1 


3.7 


9.0 


88.3 


2.0 


8.* 


89.6 


1.1 


6.1 


92.8 



CHBr 3 Layer. 


CS 2 Layer. 


CC1 4 Layer. 


2O 


30 


4 


45 


60 


8-5 


71 


91 


13 


IOO 


126 


I7-S 


130 


1 60 


22 



665 



IODINE I 



DISTRIBUTION OF IODINE BETWEEN WATER AND CARBON TETRACHLORIDE AT 25 



Results of Linhart, 19,18. 



Results of Pearce and Eversole, 1924. 



Gro. mols. I, per 1000 gms. 


c 


Gms: I 8 per 1000 gms. ^ 


7l 2 layer 7w)7 ' 


C Cl v layer (C). 


W* 


HjO layer (W). 


CCU layer (C). 


W 


o , 000402 


o . 022988 


57.2 


0.0745 


3.8990 


52.35 


O.OO0623 


0. 035260 


56.6 


O. IO2O 


5.3584 


52.53 


o . 000724 


0.040828 


56.4 


0.1078 


5.6775 


52.64 


0.000754 


O.O4302O 


57.1 


O.I432 


7.5145 


52.49 


o . 000907 


o.o5i3o4 


56.6 


0.2432 


12.6950 


52.21 



Data for the distribution of iodine between aqueous solutions of barium iodide 
and carbon tetrachloride at 25 are given by Pearce and Eversole, 1924. 

Data for the distribution of iodine between aqueous solutions of hydrobromic 
acid and carbon tetrachloride at 3o 5 and between aqueous solutions of hydrochloric 
acid and carbon disulfide at 25 are given by Ray and Sarkar, 1922. 



Data for the distribution of Iodine between aqueous solutions of 
sodium iodide (0.4933 and 0.994 RN- mols. per liter) and carbon tetra- 
chloride at 25 are given by Carter, 1928. 



DISTRIBUTION OF IODINE (WHEN AN EXCESS is PRESENT) AT 23 BETWEEN 

(SchiloVv and Lepin, 1922.) 
Water and Chloroform. Water and Toluene. 



Cms. I per 100 cc. saturated 



H 2 layer (W). 

o.o425 



CHClTayer (C). 

2.97 



c Gms.^per lOQcc. saturated T 

W " HjO layer (W). Toluene layer T. W 

70 o.o36 3.5o 97.0 



DISTRIBUTION OF IODINE BETWEEN: 

(Hcrrero, 1931, 1933* 1936.) 

Water and Carbon Tetrachloride at 20 Water and Carbon Disulfide at 25 



r*is. I per 


IJ^ter of: 


>4 layer (c) 


Hjp layer (w) x 


1.2722 


0.0169 


2.0850 


0.0273 


3,0241 


0.0391 


5.2244 


0.0651 


7.6124 


0.0938 


9.9587 


0.1199 


15-4491 


0.1825 



perj^ 



iter of; 



75-1 
76.2 

77*3 

8o.l6 

8l.l 

83.0 

84.7 



The author found that the solubility of iodine in water is not ap- 
k jreciably affected by the presence of carbon disulfide. He found 
0.2691 gms. I per liter pure water at 18 and 0.2876 gros. at 20. 
Practically identical figures were obtained when water sat. with CS g 
was used instead of pure water. 



r CS p layer (c) 


H g O layer (w)* 


w 


41.3694 


0.06979 


592 


60.1506 


0.09999 


602 


78.6780 


0.12994 


605 


85.6575 


0.14009 


611 


98.4744 


0.15862 


620 


126.1386 


0.20100 


627 


137.5596 


0.21496 


639 


152.7876 


0.23476 


650 



I IODINE 666 

DISTRIBUTION op IODINE AT 20 BETWEEN: 

(Herrero, 1933.) 



Water and Ethylene Bromide 



Water and Trichlor Ethylene 



Otas. I per liter of: 



'CHgBr.CHgBr 
layer (c) 

20. HO 
39-12 
62.46 
92,29 

12-7. U3 



H 2 
layer () 

0.03137 
0.05881 
0.09149 
0.13331 
0.18298 



650 
665 
683 
692 
696 



Gtaa. i v 


er^ liter of: 


'CCl e .CHCl 


H ? p x 


layer (c) 


layer (w) 


2.749 


O.02499 


5.098 


0.04498 


7.7^8 


0.06623 


10.872 


0.07873 


17-033 


0.14246 


22.832 


0.18870 


30.242 


0.24994 



110 
113 
117 
119 
119.6 

121 
121 



looocc sat. solution of Iodine in Ethylene Bromide contain 201.03 
gms. I at 20. 

icoocc sat. solution of Iodine in Trichlor Rthylene contain 38.78 
gins. I at 20. (Herrero, 1933.) 

DISTRIBUTION OF IODINI AT 20 BRTWBBN: 

(Herrero, 1933.) 

tfater and Benzene Water and Nitrobenzene 



Qns. I per liter of: 



'Cghglayer (c) 


H^O layer (w) 1 


12.972 


0.03499 


20.432 


0.05498 


41.240 


0.10997 


56.261 


0.1462.1 


79.984 


0.20245 


90.633 


0.22494 


97.226 


0.23869 


105.749 


0.25868 


looocc sat. 


solution of 


li V 


n M 



368 

371 
375 
385 
395 
403 
407 
409 



Gtes. I p liter of: 


layer (c) 


layer (w) 


10.28 
14.38 


0.05230 
0.07371 


19.00 
23.17 
31.06 
37.98 


0.09593 
O.ll8l5 
o. 15762 
0.19343 


44.14 


0.22532 



196 
195 
198 
196 
196 
196 
196 



solution of Iodine in Benzene contain 119.343 gms. I at 20. 
11 nitrobenzene " 56.465 " " " " 
(Herrero, 1933) 

DISTRIBUTION OF IODINE AT ROOM TEMPERATURE BETWEEN AQUEOUS STARCH 
SOLUTIONS AND CHLOROFORM. (Firth and Watson, 1922.) 

Ten cc. of a chloroform solution of iodine was shaken with 10 cc. of the starch 
solution for 10 minutes and, after separation of the two layers, the iodine remaining 
in the CH Cl s layer was determined by titration with standard thiosulfate solution. 



Gins. I per liter In ihc slarcli solution containing 



Gms. I per liter in the 
original. CHClj sol. 



0.1267 



gms. starch 


2 gms. stjirch 


j #m. starch 


i).:; gm. starch 


per liter. 


per liter. 


per liter. 


per liter. 


0.02534 


o. 015175 


0.007087 


O.O04434 


O.O228l 


o . o i i 4o5 


o.oo(5335 


0.003794 


O.O2I54 


o.oioi35 


o.oo6335 


O.003l67 


o . 02027 


o.oioi35 


0.005712 


o. oo?.534 


O.OI90I 


0.009505 


o.oo5o68 


0,002534 


o.oi584 


o.oo8:>.35 









0.1.0 1 36 
0.08869 
o . 07602 

The results show that the amount of iodino 
proportional to the concentration of the starch. 
showing the effect of various amounts of KI in the 
of iodine withdrawn from the CH C1 3 . 



withdrawn from the CH C1 3 is 

The authors also give results 

starch solution upon the amount 



667 IODINE 

DISTRIBUTION OF IODINE BETWEEN CARBON BISULFIDE AND 
AQ. POTASSIUM OXALATE. 

CDawson -Z. physik. Chem. 56, 610, '06; Dawson and McRae J. Chem. Soc. 8x, io6 s 'oa.> 



Concentration Gms. I per Liter 


O f Vol. of Solution Fraction of I 

nr V.:^l> f.n** *;.... TT n ^^nKI1 


Aq. K 2 C 2 O 4 . A Q- Layer- CS 2 L^ 01 * i Mol. I. in Solution. 

i.o Equiv. 2.408 10.82 105.3 0-005495 
i-o " 3.555 16.32 71.37 0.00561 
i.o " 5-766 27.91 43-99 0.005915 
i.o " 6.861 34-01 36.98 0-006055 

1.2 " 3.525 17.07 71.97 0.005645 

DISTRIBUTION OF IODINE BETWEEN AMYL ALCOHOL AND WATER AND 
BETWEEN AMYL ALCOHOL AND AQUEOUS POTASSIUM IODIDE 
SOLUTIONS AT 25. 

(Herz and Fischer Ber. 37, 4752, '04.) 


The original results were plotted on cross-section paper, and the 


following tables made 


from the 


curves. 








Millimols I per 10 cc 




Millimols I 


per 10 cc. of H^O and of Aq. KI Layers. 


Amyl Alcohol Layer 


f 


N 




*N 


4N 


ioN 


in Each Case. 


HzO. 


KI. 


KI. 


- KI 


KI. 


KI. 






IO 


IO 


IO 


IO 


IO 


2.5 


0.012 


0.135 


o-i 60 


0.170 


O.I70 




3.0 


O.OI4 


0-150 


0.185 


O.200 


0-2OO 


0.160 


4-0 


0.018 


O.lSo 


0.235 


0.255 


O.270 


0.240 


5 


O-O2I 


O-2IO 


0.28o 


0.315 


0-340 


0-3*5 


6 


0.025 


0.230 


0.330 


0.375 


0.4IO 


0.390 


7 


0.029 


0.250 


0-375 


0.430 


0.480 


0.470 


8 


. . . 


O.26o 


0-420 


0.490 


0-550 


0-555 


9 


. . 


O.270 


0.45 


0.550 


0.620 


0.640 


10 


. . . 


0.28o 


0.470 


0.605 


0.690 


0.720 


12 


. 


. . . 


0.490 


O.700 


0.830 


0.900 


14 






0.510 


0.790 


0.980 


i .200 


20 




... 


0-575 








Gms. I per 100 cc. 


Gms. I per 100 cc. of H 2 O 


and of KI Layers. 


Amyi Alcohol Layer 


r 


N 


aN 




4N loN 




in Each Case. 


H 2 O. 


KI. 


KI. i 


KI. 


KI. " 


KX. 






IO 


IO 


10 


IO 10 




3 


O.OI4 


0.164 


O.2O 


0.21 


0.21 




4 


0-016 


0.196 


0.24 


O.26 


0.26 o. 


21 


6 


0-026 


0.252 


0.34 


0.38 


o . 40 o . 


37 


8 


0.033 


0.297 


0-43 


0-49 


0.54 o. 


5i 


IO 


0-040 


0.328 


0.51 


0.61 


0.67 o. 


69 


12 




0.341 


0.58 


0.73 


0.81 o. 


84 


14 






0.6o 


0.83 


0.95 i- 


oo 


16 


. . . 


. . . 


0.63 


0.91 


1.09 i. 


20 


18 






0-64 




... 




25 






0.71 









The original figures for 5N/io and loN/io KI solutions give prac- 
tically identical curves. 

Results for the distribution of Iodine between N/io KI solutions on 
the one hand, and mixtures in various proportions of C 6 H 8 + CS 2 , 
C 6 H 5 CH 3 + CS 2 , C H 6 + C C H 6 CH 3 , C H fl + light petroleum, CS 2 + light 
petroleum, CS a -fCHCl 3 , CHC1 3 + C 6 H 6> CC1 4 + CS 2 and-CCl, -f C fl H 6 CH a 
on the other hand, are given by Dawson J. Chem. Soc., 81, 1086, 'oa. 



IODINE 668 

DISTRIBUTION OF IODINE BETWEEN WATER AND IMMISCIBLE ORGANIC SOLVENTS* 

Results for Water Results for Water Results for Water Results for Water 

+ Carbontetra- -1- Nitrobenzene -f- Carbon Disul- -h Chloroform 

chloride at 18. at 18. fide at 15. at 25. 

(Dawson, 1908.) (Dawson, 1908.) (Dawson, 1902.) (Hcrz & Kurzcr, 1910.) 

Mols. Iodine per Liter. Mob. Iodine per Liter. Cms. Iodine per Liter. Mols. Iodine per Liter. 



"H 2 Layer. CCU Layer. 
0.000416 0.0344 
0.000535 0.0443 

Results for Water 
4- Trichlorethyl- 
ene at 25. 
(Here & Rathmann, '13.) 
Mols. Iodine per Liter. 


H 2 O Layer. CeHaNOz Layer. H 2 Layer. CS, Layer. 
0.00019 0.0333 0.0452 27.85 
0.00050 0.0854 0.0486 30.09 
0.00133 0.2275 0.0486 30.31 
0.00189 0.3328 

Results for Water Results for Water 
+ Tetrachior- + Tetrachlor- 
ethylene at 25. ethane at 25. 
(Herz & Rathmann,/ 13.) (Herz & Rathmann, ' 13.) 
Mols. Iodine per Liter. Mols Iodine per Liter. 


H 2 O Layer. CHC1 3 Layer. 
0.00025 0.0338 
O.OOI2O 0.1546 
0.00184 0.2318 
0.00259 0.3439 

Results for Water 
4- Pentachlor- 
ethane at 25. 
(Herz & Rathmann, '13.) 
Mols. Iodine per Liter. 


' H 2 
Layer. 
0.00046 
0.00070 
O.OOII2 
0.00236 


CHCl.CCla 
Layer. 

0-0543 
0.0778 
0.1275 
0.2672 


' H 2 
Layer. 
0.00088 
0.00127 
0.00172 
0.00281 


CC1 2 .CC1 2 
Layer. 
0.0653 
0.0932 
0,1285 
0.2161 


Layer. Layer. 
0.00119 O.IIOI 
0.00145 0.1247 
0.00159 0.1479 
0.00217 0.2103 


H 2 
Layer. 
0.00092 
0.00117 
0.00160 
0.00204 


Layer. 
0.0848 
0.1067 
0.1434 
0.1963 



Data for the distribution of iodine between water and mixtures of 
at 25 are given by Herz and Kurzer, 1910. 

Data for the distribution of iodine between carbon disulfide and aqueous solu- 
tions of each of the following iodides at 25 are given by van Name and Brown, 
1917. Cadmium iodide, cadmium potassium iodide, lanthanum iodide, nickel 
iodide, strontium iodide, zinc iodide and zinc potassium iodide. Results for the 
distribution of iodine between carbon tetrachloride and aq. mercuric potassium 
iodide are also given. 

Results for distribution between CS 2 and aq. BaT 2 sols, are given by Herz and 
Kurzer, 1910. 

Data for the distribution of iodine between carbon disulfide and aqueous solu- 
tions of potassium iodide at 15 and at 13.5, and between carbon disulfide and 
aqueous solutions of hydriodic acid at 13.5, are given by Dawson, 1901 and 1902. 

Data for the distribution of iodine between carbon tetrachloride and aqueous 
solutions of mercuric bromide and of mercuric chloride at 25 are given by Herz 
and Paul, 1914. 

DISTRIBUTION OF IODINE BETWEEN CARBON DISULFIDE AND AQ. 
ETHYL ALCOHOL AT 25. (Osaka, 1903-08.) 



Cms. C>H*OH Cms. Iodine per Liter: 


f Cms. CjHsOH G ms - Iodine per Liter: 




per 100 cc. 
Aq. Alcohol. 


CSa Layer Aq. Alcohol 
c. Layer c f . 


-; per ico cc. 
c Aq. Alcohol. 


C&z Layer 
c. 


Aq. Alcohol 
Layer c'. 


c'' 


7.6 


0.072 


35-86 


0.0020 


I9.I 


0.330 


97 


0.0034 


7.6 


O.2II 


107.79 


0.0020 


22.9 


O.II5 


23-78 


0.0048 


II. 4 


0.077 


32.93 


0.0023 


22.9 


0.418 


89.61 


0.0047 


11.4 


0.280 


133-22 


O.OO2I 


26.7 


0.0756 


9.8 


0.0077 


IS-3 


0.075 


25.61 


0.0029 


26.7 


0.495 


65.10 


0.0076 


15-3 


0.315 


H5-34 


0.0027 


30-5 


0.0636 


4.90 


0.0130 


19.1 


0.045 


13.42 


0.0034 


3-5 


0.546 


42.27 


0.0129 



DISTRIBUTION OF IODINE BETWEEN ETHER AND ETHYLENE GLYCOL. (Landau, 1910.) 



* Results at o. 

Cms. Iodine per Liter: 


a 
b* 


'(C 2 H fi ) 2 
Layer (a). 


(CH 2 OH) 2 ' 
Layer (ft). 


2.139 


1.449 


1.48 


7.820 


4-347 


1. 80 


16.620 


9.486 


1-75 


20.564 


11.685 


1.76 


3L785 


18.135 


1-75 


79-950 


44.460 


1. 80 



Results at 25. 
Cms. Iodine per Liter: 


a 

r 


(r 2 H,) 2 o 

Layer (a). 


iCHaOH)," 
Layer (6). 


2.208 


1.449 *-52 


4.255 


2.541 


.60 


7.72S 


4-347 


-78 


1 6 . 200 


9.120 


-78 


30.322 


17.06.2 


.78 


78.I9S 


44-460 


.76 



669 



IODINE 



DISTRIBUTION OF IODINE BETWEEN GLYCEROL AND BENZENE AND BETWEEN 
GLYCEROL AND CARBON TETRACHLORIDK. 

.(Landau, r<ito.) 



Results for Glycerol and Benzene. 



Results for Glycerol and 



^*- Glycerol Layer, 
(a) 


Benzene Layer. 


vw; 
(a)' 


t (jiycerol Layer . 


CCU Layer. 
<*) 


(>' 


25 


0.407 


1.922 


4.72 


25 


0.365 


0.565 


1-55 


a 


0.676 


4.086 


6.04 


a 


0.684 


I .224 


1.78 


tt 


1.470 


IO.2I2 


6-95 


tt 


I .416 


2.652 


1.87 


" 


2.622 


2O. 102 


7.67 


tt 


5.064 


9.888 


i .95 


u 


5.280 


42.458 


8.04 


tt 


7.636 


14.766 


*-93 


40 


0-459 


2.168 


4.72 


4 o 


0.322 


0-575 


1.79 


tt 


0.658 


3.911 


5-94 


u 


0.690 


1.169 


1-74 


tt 


1-5^4 


11.244 


7.10 


tt 


1.224 


2.772 


1.69 


" 


3.048 


24 . IO4 


7.91 


tt 


2.832 


6.444 


2.26 


a 


5-564 


46 . 960 


8-44 


a 


& 6.854 


15.410 


2.25 


s 


0.467 


2.194 


4.70 


50 


O.299 


0.653 


2. 19 


tt 


0.642 


3.864 


6.02 


tt 


0.570 


I .270 


2.23 


it 


1.463 


II .196 


7.65 


tt 


I-5II 


3-457 


2.29 


tt 


2.391 


19.872 


8.31 


tt 


2.664 


6.468 


2-43 


it 


5-333 


46.782 


8.69 


tt 


6.348 


16.008 


2.52 



DISTRIBUTION OF IODINE BETWEEN GLYCEROL AND CHLOROFORM. 



Results at 25. 
(Herz & Kurzer, 1910.) 

Mofs. Iodine per 1000 
Gms. c 


Results at 30. 
(Hantzsch & Vagt, 1901.) 

Mols. Iodine per Liter: 


t. 
o 

20 
40 
50 


Results at Dif. Temps. 
(Hantzsctt & Vagt, 1901.) 

Mols. I per Liter: 


'Glycerol CHC1 3 c' 
Layer c. Layer t r . 
0.0244 0.0564 0.43 
0.0397 O.ogiQ 0.43 
0.0500 0.1151 0.43 


(Jlycerol CHCU c' 
Layer c. Layer c'. 
0.00097 0.00172 0.056 
O.O0204 0.00412 0.495 
0.00418 0.00898 0.465 

0.00782 0.0216 0.362 


Glycerol CHCI 3 c' 
Layer c. Layer <;'. 
0.0119 0.0177 0.675 
0.0084 0.0213 0.400 
O.OO77 O.O22I 0.349 

0.0074 0.0226 0.330 



Data are also given by the above named investigators for the distribution of 
iodine between aqueous glycerol solutions and chloroform at several temperatures. 

DISTRIBUTION OF IODINE BETWEEN GLYCEROL AND ETHYL ETHER. 

(Hantzsch & Vagt, 1901.) 
Mols. Iodine per Liter: 



t*. 

o 


Glycerol Layer 
(c). 
0.00566 


Ether Laver 
(c'). " 
O.O27O 


c'" 
O.2I 


30 


0.00544 


O.O272 


O.2C 


30 


O.OOIQO 


O.OO5I 


O.2O 



I IODINE 670 

SOLUBILITY OF IODINB IN LIQUID CARBON DIOXIDE. 

(Qulnn, 196.) 



d of 
C0 



Eat. density 
of aat. aol. 



-31 1.031 (-20) 1.031 (-30) 

-11.4 0.981 (-10 ) o.982(-io ) 

o 0.927 0.929 

+10 0.858 0.863 

20 0.770 0.775 

35 0.710 0.720 



Ota. I por 
0. Mol. 00 p 

. 01 02 
0.0191 
0.0347 
0.0526 
0.0774 
0.0915 



dna. I pr 
100 gn. Q0 2 

0.0232 
0.0434 
0.0788 
0.1195 
0.1759 
0.2079 



SOLUBILITY OF IODINE IN CARBON BISULFIDE. 



t e . 

-100 

- 80 

- 63 

- 20 

- 10 



Cms. I per 100 
Cms. Solution. 

0.32 
0.51 
1.26 
4,14 
5-52 



(Arctowski, 1894.) 

AO Gms. I per 100 
Gins. Solution. 

o 7.89 
10 10.51 

15 12-35 
20 14.62 
25 16.92 



30 
36 
40 
42 



[Gms. I per too 
Gms. Solution. 

19.26 
22.67 
25.22 
26.75 



SOLUBILITY OF IODINE IN SEVERAL SOLVENTS AT 25. 



Solvent. 

Chloroform 

Carbon Tetrachloride 

Tetxachlorethylene 



(Herz and Rathmann, 1913.) 



Iodine per Liter of 
Sat. Sol. 


Solvent. 

Trichlorethylene 
Tetrachlorethane 
Pentachlorethane 


Iodine per Liter of 
Sat. Sol. 


" Mols. Gms. 
0.352 44.68 
0.237 30.08 
0.241 30.59 


Mols. Gms. 
0.312 39.61 
0.244 3-97 
0.272- 34.53 



SOLUBILITY OF IODINE IN SEVERAL SOLVENTS. 

(Margosches, Hlnner ana Frledwann, 1924.) 



One. I per lOOcc sac. solution In: 



c 


' Carbon 


Chloro- Methyl en e 


Tetra chloro 


Trl chloro 


Dl chlor x 




Tetrachlorlde 


form Chloride 


F.chylene 


Echylene 


Ethylene 




cci 4 


<C1 5 CH^Clj, 


CCl ? .CCl p 


CHCl.CClg 


CH ? CC1 R 


11 


1 .77 


2.84 3.68 


1.87 


2.48 


2.99 


15 


2.05 


3.2C 4-. 22 


2.10 


2.80 


3.38 


18 


2.25 


3-54 4.65 


2.32 


3-05 


3-72 


21 


2.51 


3-95 5-13 


2.59 


3-41 


4-13 


25 


2.91 


4.52 5-86 


3.06 


3-96 


4.76 




Ctas. I per 100 cc sat. solution in: 




t 


' Pencachloro 


Acetylene 


Chloro Ethyl en e 


Echylene 


Ethylldene 




Ethane 


Tetra Chloride 


Chloride 


Chloride 


Chloride 




CHC1 ? . CClg 


CHCl ? .CHCl g 


CH 2 .CHd 


CH,C1.CH,C1 


CH 3 .CHC1 2 


11 


2.02 


2.71 


3-72 


4-59 


3.00 


15 


2.31 


3-01 


4-15 


5.11 


3-25 


18 


2.50 


3-22 


4-50 


$.59 


3-49 


21 


2.80 




4.91 


6.13 


3.92 


25 


3-09 


4.10 


5-47 


6.87 


4-39 



6 7 l 



IODINE I 



SOLUBILITY OF IOBINB IN SEVERAL SOLVENTS. 



Ftormula 



dns. Iodine per 

< . A 

100 gns. 100 cc s 

sat. sol,, sac. sol. 



Auchorlty 



Acetic Acid 



20 1.727 

11 " " 30 2,706 

"Bthyl Ester CILCOOCJL 8 11.1 

" 11 12.39 

" " " " 30 16.15 

Carbon DisuUide CS 25 

Carbon Tetrachloride CCl A o 

11.5 

" " " 25 

Tetra chlor ethane CHCl p .CHCl 8 25 



Bromoforn 


ClfBr g 


^ 5.6 


3.22 


HI 


n 


25 


6.6 


II 


M 


25 





Benzene 


C 6 " 6 


25 





H 


II 


20 


8.15 


" 


H 


30 


11 .64 


Nitrobenzene 


C 6 H B N0 8 


16-17 





Toluene 


C Q !I 5 Cff 3 


25 





Hexane 


CH 8 (CH 8 4 CH 8 


25 


12.2 


Anhy. Lanolin 


(m, pt. 46 ) 


45 


5-5 



(Anders, 1933.) 

(Knott,- 1932.) 



23.0 (Jakowkin, 1895 

1.04 (Grohj 1927-) 
1.83 

3.03 (Jakowkin, 1895 

4,16 ( Grace ? 1931.) 

(Amadori, 1922. 

ITurner and 



19 iff* ) 

18.96 (Jakowkin, 1895.) 
13*83 (Grac^, 1931.) 

(Anders, 1933. ) 

~~~ H 

5.06 ( Dawson and (jaw lor, 
1902- ) 

3,56 ( Sc h i low and Lep i n 
1922. 1 

(Hildebrand and 

Jenks, 1920,1 

{ Klose, 1907. ) 



SOLUBILITY OF IODINE IN CARBON TETRACHLORIDE. 

(Jacek, 192(1; Hildebnmd and Jenks, 1920.) 



Gins. I 


<; 


ins. I 








t. 


per JO') gins. C Cl,. 


t". 


IHU- 100 


gins. Cl,. 




t". 


-24. 


7 5... 


O 


.254 


- 16 


. 5 . . . . 


O. 


,1)2 


- 17 


>* 


-24 


o 


Q 


>5 r 7 


r 'i 


,.- 




i ;- 


/. 




->n . 
-22. 


o 


O. 


1 ZJ y 
,270 


i ,.j 
-LI 


.25. . . 


o. 


447 


- 2 


.o(. . . . 

.75 .... 




I Q 


o 


o 


2U7 


... Q 


. 5 .... 


Q 


460 






-is! 


5.... 


0. 


^yy 
,819 


.7 

- 8 


. 5 .... 


o. 


48o 


O 


. o ..... 


-17. 


o. . . . 


o. 


,327 


- 8 


.25 . . . 


o. 


4<)() 


35 


















* j 


5< 


.0 



!rH.;mU. 



SOLUBILITY OF IODINE IN CARBON BISULFIDE. ( Jacek, itur*. ) 



finis. I 
t- per 100 gins. CS 3 . 

-107 o.i 58 

- 80 0.255 

- 77.5 o.34:>. 

- 71.5. ... 0.422 



-5 1 ...... . 

-45 ....... 

35.2'), . . . 



Cms. ! 
iuo ^ins. C 

0.520 

1.089 
' 




I IODINE 



673 



SOLUBILITY OF IODINE IN CHLOROFORM. 

( Below ? Jacek, 1915 ; above 0, Grimbert, Malmy and Poirot, 1924 ; Malmy, 1926. } 



f. 
-60 


Cms. I 
per 100 gms. 
CHC1 3 . 

0.089 
0.128 

0.180 

0.243 
0.372 
0.404 
0.514 


t. 
q c 


Gms. i 
per 100 gms. 
CHC1 3 . 

).856 
.o54 
.198 (M.) 
.240 
.237 (M.) 
.267 (M.) 

.483(<;. M. and P.) 


t. 
IO . . 


Cms. T 
per 100 guis. 
CH Cl a . 

I.8o5(G. M. andP.> 
2.176 
2.533 )) 

2.63o )> 
3 . 092 
3.2oo(3.38*) 
3.836(M.) 


-5 1 


-5 


i5 

IQ . . 


-45.5 


-i .... 


-35.o 
-3o 


o 

o 


20 

>/ 


-25 


+o.5... 
5.o... i 


25..... 

3o 


-22.25 



* Gms. per 100 cc. sat. sol. at 25 ( Schilow and Lepin, 1922. ) 

too gms. chloroform for anasthesia, containing o.oo5 per cent C a H 5 OH, dissolve 
2.19 gm. I at 15. (G. M.andP.), 

SOLUBILITY OF IODINE IN ETHYL ETHER. ( Jacek, 1915. ) 



i - 





Gms. I 




Gms. I 




Gms. I 


t n . 


per iot> gms. 
(C 8 H 3 ),0. 


r. 


per 100 gms. 


v. 


per lOOgras. 
(CH S ),0. 


108 


i5. 10 


5i 


ifi // 


__2 jr 


3ft 


94.5.... 


i5.43 




17.08 


T C\ ^ 


2O. ,38 


jyi . \f . 








1 \) . J . . . . 




83.25... 


15.46 


4o.25 .. 


17.67 


T4.75... 


21.39 


75 


15.67 


3/i 75 


18.64 






63 


16.16 


vq. . J^i . . . 

-24.5.... 


19-67 







SOLUBILITY OF IODINE IN HEPTANE. ( Hildcbrand and Jenks, 1920. ) 



t". 
o 


Gms. I 
per 100 gms. sat. sol. 

o 6176 


Mols. I, 
per 100 mols. sat. * 

o.oo->.45 
0.006786 
0.00998 
o orfion 


90l. 


25 




35 




5o 


4.IQ6 



SOLUBILITY OF IODINE IN BENZENE, CHLOROFORM, AND IN ETHER. 

(Arctowski Z. anorg. Chera. n, 276, ' 



In Benzene. 


In 


Chloroform. 


In Ether. 


f. 


Gms. I per 100 
Gms. Solution. 


t". 


Gms. I per 160 
Gms. Solution. 


t c . 


Gms. I per TOO 
Gms. Solution. 


4-7 


8.08 


-49 


0.188 


"83 


15-39 


6.6 


8.63 


*"Ss4 


0.144 


-90 


, X 4-S8 


10.5 


9.60 


-60 


0.129 


-108 


15.09 


13-7 


10.44 


69 j 


0.089 






16.3 


11.23 


-73i 


O.o8o 







+ 10 i .76 per 100 gms. CHCla 

(Duncan Pharm. J. Trans. 22, 544, 



673 IODINE I 

SOLUBILITY OF IODINE IN ACETONE AND IN BENZENE. 



Results for Acetone. 

(Jacek, 1915.) 



81... 


Cms. I per 100 gms. 
CH 3 .CO.CH S . 

->.73 


f. 
34. . . 


Cms. I per 100 gins. 
CH 3 .CO.CII 3 . 

6 54 


c 

t. 

25 


75. . . 


6 76 


3o. , 


5 3o 


3o . 


70.5. 


.. 8.83 


22 . 5 . 


4.5 




54.75 


1 5 . 06 


18.0 


4*^5 


/ o 


53.0. 


. . i3.5 


16.0, 


3.9 


45 




12. I 




2.66 




44.5. 
-42.0. 


.. 8.6 
.. ' 8.6 


o.o. 


2.56 


54.64.. 



Results for Benzene. 
(Hildebrand and Jenks, 1920.) 

Cms. I per 1 00 gros. Mols. I 8 por 1 00 
sal, sol. 

14.09 

l6. IO 
17.90 



mols. sat. sol. 
O.O 4 80 

o.o558 
0.06-29 
0.0716 



28.26 



0.0953 
o . 1 08 1 



SOLUBILITY op IODINE IN SEVERAL SOLVENTS. 

(Neglshlf Donnelly and Hlldebrand. 1933.) 



Solvent 



Titanium tetra chloride, TiCl 4 
n n n H 

II M II II 

Silicon tetra chloride, SiCl 4 

ti n it it 

Ethylene Bromide, CH 2 Br.CH 2 Br 



Iso Octane, CH_CICH,) P CM P CH 

tCH,) CHj 
(2.2.4-tri methyl pentane)" 





fas. I per 


Ota. Mols. Ip per 


* 100 


gwa. sac. sol. 


100 0*. mols. sat. sol. 


0.1 


1.153 


0.8633 


25.0 


2.855 


* 2.150 


40.0 


4.631 


3.499 


49*9 


6.500 


4-939 


0.1 


0.2555 


0.1713 


25-0 


0.7433 


0.4987 


40.0 


1.309 


0.8801 


8.0 


6.557 


4.925 


10.0 


6.850 


5.161 


15.0 


7.859 


5.937 


20. 


9.091 


6.895 


25.0 


10.32 


7.815 


35.0 


13.42 


10.28 


45o 


17.43 


13-51 


49.6 


19.12 


14.89 


60.0 


25-54 


20.24 


70.0 


33-30 


26.97 


75-0 


37.6i 


30.85 


73-4 


42.40 


35.26 


24.92 


1-302 


0.590 


35-0 


1.918. 


0.8711 



deter- 



In the cases of the titanium and silicon tetracJiloride the 
minations *ere made in an atmosphere of nitrogen. 

SOLUBILITY OF IODINE IN NORMAL PENTANE AND IN Iso PENTANE. 

(Jacek, 1926.) 

Results for Normal Pentane. Results for Iso Pentane. 



P 


Cms. I 
er 100 gms. 


Gms. I 
per 100 gms. 


Gms. I 
per 100 gms. 


Gms. 1 
per 100 gms. 


t*. cn 3 (Cir s ) 3 crr 8 . 


f. CH 3 (CH 8 ) 3 Cir s . 


t'. (CI) 


r a )sCrrcH a cir u . t'. (cn a ) s ciicn t cir,. 


-71.25.. 


0.018 


-26.75.. 


o. 160 


-79.25.. 


o 017 


-3i.5. .. 


o. 117 


-69.75.. 


O.O2I 


-26.0,.. 


o. 171 


-66.25.. 


0.018 


-25.25.. 


o.i55 


-54.25.. 


. 042 


-i5.25.. 


0.297 


-56.0O. . 


o.o33 


-23.5... 


o. 172 


-48.75.. 


0.057 


- 7.0. . . 


0.423* 


-49 o... 


0.039 


-2 I . O . . . 


O.2OO 


-45.25.. 


0.067 


- 5.5... 


o.483 


-^2.5... 


o.o63 


-IO.O. . . 


0.345 


-40.75.. 


0.078 


o.o. . . 


o.6o5 


-37.5... 


o . 080 


- 8.0... 


o.38i 


-34 25.. 


o.n3 


+19.0... 


1.377 


-36.95.. 


0.089 


- 8.0... 


0.375 










-34.25.. 


0.096 


. . , . 


o . 562 



674 

I IODINE 

RECIPROCAL SOLUBILITY OF IODINE AND SULFUR IN BENZENE 

AND IN CARBON BISULFIDE AT 25. (Amadori, 1922.) 
Results for Benzene. Results for Carbon Disulfide. 

Gins, per 100 gms. sal." sol. Gnk per 100 gins. sat. sol. 

I. S. Solid Phase. I. S. Solid Phase. 

15.79 o.o I 19-14 o.o I 

16.08 0.40 19.83 7.76 

i6.-z8 1.75 Jto.fi.i 12.83 

16.4-2 2.58 I-t-.S iu.45 27.78 

12.72 2.4'2 S 24.ii 86.74 

8.3l 2.35 22.64 40.82 S-I-I 

o.o 2.09 16.08 39.56 S 

9. -4 37. 12 

6.62 86.42 

o.o 34^76 

Data for the reciprocal solubility of iodine and sulfur in carbon disulfide at 10 

and at 18 are given by Mori, 1923. This author also found no evidence of the 

existence of compounds of iodine and sulfur, 

Bromolorm simultaneously saturated with iodine and sulfur contains 3.7 gms. I 
and 4.2 gms. S per 100 gms. sat solution at 3.65. (Amadori, 1922.) 

r 



.RECIPROCAL SOLUBILITY OF IODINB AMD SULFUR IN CARBON TETRACHLORIDB. 

(JaK.owK.in anil Arkhangelsk^,, 1936.) 

Results at o Results at 25 

OBIS, per lOOqp sat., sol. Solid Gtas. per lOOcc sat. sol. SolM 

t . j Phase * I s * F'h*se 

1.145 0.0 I 2*905 0.0 I 

1.157 0.$<;6 I + S 3.083 i.fj66 I + S 

0.818 0,596 S 2.069 1.105 S 

o.o 0.596 S 1.998 1-394 S 

o.o 1.329 S 

Solubility results an mixtures of Iodine and Potassium Iodide with 
Chloroform and with Toluene, j{iven by Foote and Bradley, 1932, show 
that between 0.7 and 25.0 no solid binary addition product of Iodine 
and Potassium Iodide exists. With benzene a ternary addition product 
having the composition KI.nl ? .^C^ Q was found. 



6 75 IODINE I 



SOLUBILITY OF IODINE IN NITROBENZENE SOLUTIONS CONTAINING VARIOUS 
IODIDES AT ROOM TEMPERATURE. SOLUTIONS SAT. WITH 1 IN EACH CASE, 

(Dawson and Goodson, 1904.) 

Oms. per Liter. _ ,. , Cms. per Liter. 

Iodide. - rr; * rr Iodide. * ,. . * v .. > 

Iodide. iodine. Iodide. Iodine. 

Potassium Iodide 12.35 112.7 Caesium Iodide* 48.2 213 

" " 45.56 295.7 Caesium Iodide 223 858 

" " 115.8 698.2 Ammonium Iodide 69.5 482 

" " 155-2 943-6 Ammonium Iodide* 04-3 M>g 

Sodium Iodide I 3-55 I2 5 Aniline Hydriodide 164 721 

" " 57.7 393 Dimethylaniline Hydriodide 160 626 

" " 109.1 738 Tetramethylammonium Iodide 40 -3 266 

" " 228 1251 Tetramethylammonium Iodide ST. 4 280 

Rubidium Iodide 85.4 421 Strontium Iodide 106.5 599 

Rubidium Iodide 217.5 IQ 6o Barium Iodide 42.2 237 

Lithium Iodide 84.1 642 Barium Iodide 158.5 809 

* Solvent = o nitrotoluene instead of nitrobenzene. 

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 OK IODINE IN MIXTURES OF SOLVENTS AT 25. 

(Mahleu, 1336.) 
In Ether -* Chloroform In Methyl Alcohol -f Chloroform 



Oms. (CpH^pP per 


Oms. I per 100 gras. 


Ctas. OHOl^ per 


'Oto a. I per 10O gins. 


100 gjafl. solvent mixture 


solvent mixture 


tOO tsns. solvent mixture 


solvent mixture 


o.o(= CHC1 3 ) 


2.01 


o.o( = CH 8 OH) 


2335 


25.1 


4.80- 


2/|.l 


17-97 


48.1 


7.34 


50.3 


12.75 


73.6 


15.03 


74-4 


7.71 


100-0 


23.86 


1OO.O 


2 . 11 



SOLUBILITY OF IODINE IN MIXTURES OF ACETIC ACID AND BENZENE, 

(Anders, 1333.) 

Results at o Results at 20 Results at 30 

Qms. CH,COOK Qms. I per Qms. RH,COOH Gtas. I per rkis. CH.CQOH Hma. I yr 

o o o 

per 100 gms. 100 gms. sat. per 100 gms. too gma. sat. per 100 tfms. 100 BBS. aat. 

solvent mlxorre solution solvent mixture solution solvent mixture solvent 

21.788 3.892 o.o 8.152 o.o 11.642 

47.961 3.1S6 21.516 7.107 21.371 9.745 



I IODINE 676 

SOLUBILITY or IODINE IN MIXTURES OF CHLOROFORM AND ETHYL ALCOHOL, 
CHLOROFORM AND NORMAL PROPYL ALCOHOL, CHLOROFORM AND BENZENE, 
AND CHLOROFORM AND CARBON DISULFIDE AT 15. 

(Bruner, 1898.) 

Vol ^ CHC1 Cms. I Dissolved per 100 cc. of Mixtures of: 

insolvent. 3 ' "* 

O 
10 
20 
30 
40 

So 

60 
70 
80 

go 

IOO 

SOLUBILITY OF IODINE IN MIXTURES OF CARBON TETRACHLORIDE AND BEN- 
ZENE AND IN MIXTURES OF CARBON TETRACHLORIDE AND CARBON DISUL- 
FIDE AT I 



CHC1 3 +C 2 H 5 OH. 


CHC1 3 +C 3 H 7 OII. 


CHC1 3 +C 6 H 6 . 


CHCl 3 +c. 


I5-67 


14-93 


IO.4O 


17.63 


9-43 


13.16 


9.84 


J 5-93 


8.69 


II. 2O 


8.78 


14.20 


7.80 


8.98 


7-74 


12. l6 


7.09 


8.09 


6.96 


IO.2O 


6.62 


7.82 


6. 20 


9.08 


6.24 


7.09 


5-34 


7.72 


5-77 


6.42 


4.89 


6.42 


5-06 


5-54 


4-53 


5-27 


4/34 


4-52 


4.07 


4-32 


3.62 


3.62 


3.62 


3.62 



Vol. % CC1 4 Gms. I per ioo cc. of Mixture of: y Q j ^ ^\ Gms. I per 100 cc. of Mixture of: 

in ^ lvent ' ' CC14+C.H* *" CCU+CS,. * insolvent/ *" 



o 10.40 17.6 60 4.90 5.55 

10 9.44 14.44 70 4.09 4.50 

20 S-53 12.33 80 3.41 3.37 

30 7-77 *-34 9 2.74 2.60 

40 6.63 8.60 loo 2.06 2.06 

So 5-70 6.83 

In the case of the above determinations the volume change occurring on mixing 
the solvents w.as neglected. The temperature was not accurately regulated and 
the mixtures not shaken during the saturation. The curves plotted from the 
results are not smooth. 

SOLUBILITY OF IODINE IN MIXTURES OF CHLOROFORM AND ETHER AT 25. 

(Marden and Dover, 1916.) 

Cms. CHCU per ioo. Cms. Iodine per 100 Cms. CHC1 3 per 100 Gms. Iodine per too Gms. 

Gins. CHC1 3 +(Q 1 H 6 ) 2 0. Gms. CHClj-KQH^O. Gms. CHC1 3 +(C 2 H 6 ) 2 O. CHCI 3 -KC'Hi) 2 0. 

o 35.1 60 9.83 

10 29.6 70 7.5 

20 24.8 80 5.73 

30 20.2 90 4.31 

40 16.3 ioo 3.10 

50 12.7 

ioo cc. of a mixture of CHCls 4- CSa (3:1) dissolve 7.39 gms. iodine (t ?.) 
The addition of S even up to the point of saturation does not affect the amount 
of iodine held in solution. (Olivari, 1908.) 

Diagrammatic results for mixtures of iodine and each of the following com- 
pounds are given by Olivari, 1911: CHI 3 , p C rhBr 2 , [CcH 4 ]N 2 , p Ce 
(CH 6 CO) 2 and C 6 H 6 COOH. 



677 



IODINE I 



SOLUBILITY OF IODINE IN 


MIXED SOLVENTS AT 16.6. 




(StrSmholm, 1903.) 




Gms. I 




Gms. I 


Solvent. 


per Liter 


Solvent. 


per Liter 




Sat. Sol. 




Sat. Sol. 


Ether 
Carbon Bisulfide 


206.3 
178.5 


Ether 4- 20.96 gms. CSj per liter 
Ether-hH-9 " CS 


202.3 
217.2 


Ether4-3-96 gms. H 2 O per liter 


221 


CSa 4-22.5 " ether " 


189.3 




4-7-Qi gms. H 2 O " 


235-7 


CS 2 4-45-1 


' ether " 


201. 1 




4-excess HaO 


251.4 


Ether 4-47-63 


1 CHCls " 


195.2 




4-9-79 gms. C 2 H 6 OH " 


2I9.I 


82 4-50-06 


' CHC1 8 " 


172.8 




+19.6 " 


231,5 


Ether4-8o.3 


4 C 6 H 6 " 


204.1 




4-29.4 " " " 


243-9 


Ether-j-77-8s 


1 CH 3 I " 


220.2 




4-39.2 " 


254.4 


CS-2 +62.2 ' S 


189.4 



One liter sat. solution in ether contains 167.3 gms. I at o. (StrSmholm, 1903.) 



SOLUBILITY op IODINK IN CARBON TBTRACHLORIUB CONTAINING OTHER SOLVENTS. 

(Oroh, 1927.) 



Results for Carbon Tetrachloride containing: 
Methyl Alcohol Ethyl Alcohol 



Propyl Alcohol 





On. Mola 


. per liter 


On. Mols. 


per liter 


Gto. Mols. per liter 


t 


sat. sol.^ln CC1 4 


t sat. sol. 


A ln CCI 4 


t sat. aol^ 


In CC1 4 




' CHgOH 


x a V 


'CgHgOH 


T 2 X 


' C &7" 


F ? ' 





0.192 


0.0524 


o 0.205 


0.0556 


o 0.208 


0.0547 


it 


0.^11 


0.0601 


" 0.410 


0.0653 


11 0.414 


0.0636 


M 


0.6l7 


0.0673 


" 0.609 


0.0741 


11 0.622 


O.O721 


" 


0.8l4 


0.0743 


" 0.808 


0.0829 


" 0.815 


0.0800 


it 


0-993 


0.0806 


" 1.025 


0.0924 


" 1-035 


0.0889 


" 


1.234 


0.0891 


" 1.232 


0.1015 


11 1-307 


0.1001 


it 


1.607 


0.1022 


1.621 


0,1193 


1-543 


0.1096 


" 


2.032 


0.1168 


" 2.013 


0.1365 


" 2.045 


0.1312 


11. 


8 0.188 


0.0816 


11.7 . 20 1 


0.0849 


11.6 0.198 


0.0835 


n 


0.404 


0.0920 


11 0.404 


0.0970 


" 0.403 


0.0947 


lv 


0.596 


0.1006 


0.596 


0.1080 


11 0.594 


0.1051 


" 


1.011 


0.1191 


0.807 


0,1202 


0.805 


0.1163 


it 


1,120 


0.1237 


11 1.010 


0.1319 


" 1.005 


0.1267 






Acetic Acid 






Ethyl Ether 




r o 


Om. Mols. per liter^at. sol. In CCl^ 




Mols. per ilter^sat 


. sol. in CCl^ 


t 


f 


CH^OOK 


! ? 


t / 


<W? 


'* 







0.0 


0.0450 





0.211 


0.0549 


n 




.201 


0.0464 


n 


O.422 


0.0650 


it 




0.395 


0.0477 


it 


0.633 


0.0748 


it 




0.797 


0.0501 


" 


0.844 


0.0853 


ii 




0.992 


0.0513 


it 


1.055 


0.0960 


tt 




1.148 


0.0522 


it 


1.266 


0.1063 


11. 


15 


0.204 


0.0715 


11.4 


0.0 


0.0710 


11 




0.406 


0.0730 


n 


0.196 


0.0815 


n 




0.547 


O.0744 


n 


0.390 


0.0927 


n 




0.897 


0.0765 


it 


0.585 


0.1037 


n 




l.lSl 


0.0786 


n 


0.865 


0.1206 










n 


1.171 


0.1399 



I IODINE 678 

MUTUAL SOLUBILITY OF LIQUID IODINE AND CARBON TSTRACHLORIDE, 

(HHdsbrand, 19.T7.) 

The determinations were made by the synthetic method but due to the 
opacity of concentrate iodine solutions advantage was taken of the 
difference in density of the two liquid phases for detecting their 
points of separation. 



o 


Wt f. 


Mol * 


ut 


Mol'% 


t 


Iodine 


Iodine 


c ' Iodine 


Iodine 


128.8 


44.8 


33-0 


160 -5 (max.) 


67*0 


155.0 


63.0 


50.8 


160.1 80.8 


71.8 


158.1 


67,0 


55.1 


159-9 81.7 


73-1 


160.6 


76.0 


65.7 


153*5 86.6 


797 



SOLUBILITY OF IODINE IN ARSENIC TRICHLORIDE. (Sloan and Mallet, 1882.) 

t. 0. 15. 96*. 

Cms. I per 100 gms. AsCI 3 8.42 1 1 . 88 36 . 89 

FREEZING-POINTS OF MIXTURES OF IODINE AND IODOFORM. 

(Vasilev, 1916.) 

I content of mlxt.ire. I conlcnt of mixture. 

t". Wt. / u . Atom / . Solid Phase. t- Wt. / . Atum/ . Solid Phase. 

I l4. <>.- KJO. 100. I (if) . I (Eiitee.). ,(>.. 3 - I-fClII 3 

<)7.8... 87.84. cf>.70 > 70.9...... 38.85 6633 GHI 3 



94.8 85.38 94. 8 

79 8 70. aa 87.98 

73.6 59.41 81.96 

71 .2. ... 53. 3o 77. (}(] 

69.:). . . . 49.08 



78.1 3i.45 58.76 

8f>. ^.4.63 5o.35 

95 . 8 1 7 . 63 39 . 4 ( > 

111.9...... 5. '^.o i4.55 

119.7...... o . o o . o 

Similar data for iodine + naphthalene gave a single eutectic at 65.7 and 
39.43 wt. % I. 

Fusion-point data are given for the following mixtures: 

I -4- As (Jaeger and Doornbosch, 1912,) 

I + Cal p (Olivari, 1908.) 

I + H ? I f 

I la (Thiel and Koelsch, 1910.) 

I * KI (Olivari f 1914; Brigfjs and Geigle, 1930; Fialkovf and 
Kensmenkc, 1936.) 

I * Lil (Fialkow and Kensmenko, 1936.) 

I + S (Olivari, 1908; Boulouch, 1903; Smith and Carson^ 1908-) 

I # Sb (Jaeger and Doornbosch, 1912.) 

I + Se (Pellini and Pedrina, 1908.) 

I + Sn (Van Klooster, 1912-13; Reinders and Lange, I9i2-*i3; 
Vasileu, 1916, 1917.) 

I -f te (Jaeger and Menke, 1912; Damiens, 1921, 1923*) 

I 4- Tl (Fialkow and Kensinenko, 1936.) 

I + Each of the following compounds: Azbbenzene, benzole acid, 
Benzole anhydride, Dibrom benzene, Dinitrobenzene* lodoform, 
Tetra methyl ammonium Iodide and Tri methyl phenyl ammonium 
iodide. {Olivari, 1911.) 



679 SOD I HE I 

IODINE CYANIDE ICN 

One liter sat. solution of iodine cyanide in water contains 0.2523 
gm. mols. at 25. (Yost and Stone, 1933.) 

DISTRIBUTION OP IODINR CYANIDE BETWEEN WATER 
AM) CARBON TBTRACHLORIDB AT 25 

(Yost and Stone, 1933.) 
In. Mols. ICN per liter of: c 



/H ? layer (w) CC1 4 layer (c) ^ " 

ON 
0.02^80 0.00/^60 0.1798 

0.03312 0.006007 0.1814 

0.05144 0.009441 0.1835 

0.06697 0.01239 0.1850 

0.07960 0.01482 0.1862 

IODINE PBNTOXIDE I,0 S . 

SOLUBILITY OF IODINE PENTOXIDE IN SULFURIC ACID AT 2i.77, 
(Lamb and Phillips, 1923.) 

Constant rotation in a thermostat was employed. Equilibrium was reached 
in some cases within one day, but with higher concentrations of sulfuric acid, there 
was a slow decrease from a definite initial solubility. This was studied over a 
period of 55 days and constancy was reached in all cases within 4o days. 

For cent Gms I S 5 per liter Per cent Gms I 9 5 per liter 

H S SO,. Initial. Final. ll a SO*. Initial. Final. 

5o.o 54./9 54-79 89.0 >.>,. i i.5. i 

(>o.o. 34-68 34.68 90.3 iw-7 i4.5 

75.o 19.48 19.48 92.0 23.4 i *. 5 

78.0 i8.(6 18.66 96.0 (-.43.2) n.o 

79.6 19.0 18.5 98.0 (>/>,. o) 9.5 

82.0 19.9 18.8 99.9 - 3.48 

84. (> '2<).'5 19.3 102.0* - 1.28 

86. o 21.0 17.1 104.0 - 1.90 

87.4 21.5 i5.8 io(>.o - -2.(>7 

* This perceiitage represents weights of 100 % H S SO, equivalent to 100 gm. of the add in ques- 
tion. The 106.5 /o of acid, therefore, contained 29.0 % of free S0 a . 

INDIUM la 

SOLUBILITY OF INDIUM IN MBRCURY. 

(Parks and Mo ran, 19.77.) 

Qtos. Tn per Ghi. Atoms In per 

C IOC 0aa. Tn Hg loo. ens. Ato8 In * Hg 

1.23 2.14 

12.5 1.27 2.20 

25 1.26 2.l8 

37-5 1.2S 2.22 

SO 1.31 2.27 



INDIUM IODATE In(IO 3 ) 3 . 

100 gms. H 2 O dissolve 0.067 gm- In(I0 3 )3 at 2O. (Mathers and Schluederberg, 1908.) 



Ir IRIDIUM 68o 

INDIUM Ammonium SULFATE In (NH J JSO J .248 

* 4 P 442 

100 gms. H p O dissolve 200 gms. of the salt at 16 and 400 gms. at 
30. (Rossler, 1873. * 

IRIDIUM CHLORIDE IrCl 4 . 

When i gm. iridium as chloride is dissolved in 100 cc. of 10% HC1 and shaken 
at 1 8 with loo cc. of ether, 0.02 per cent of the metal enters the ethereal layer. 
When 20% HC1 is used 5% of the metal enters the ether. When dissolved in i % 
HC1 or in water approximately o.oi per cent of the metal enters the ethereal layer. 

(Mylius, 1911.) 
IRIDIUM Potassium CHLORIDE IrK^Clg 

100 gms. H ? dissolve 1.25 gms. IrK,,Cl ft at 18-20. 

100 gms, H.,0 dissolve 9.18 gms. dipdtassium aquo penta chloroiridite, 
IrCl c (H ? 0)Kj,'at 19. (Delepine, 1908.) 

IRIDIUM Ammonium CHLORIDE IrCl 4 .2NH4Cl. 

SOLUBILITY IN WATER. 

(Rimbach and Korten, 1907.) 
Gms. IrCl 4 .2Nft 4 Cl per 100 Gms. Gms. IrCl^NHiCl per 100 Gms. 

Water. Sat. .Sol. " ' W^ter. Sat. Sol. 

14.4 0.699 0.694 52.2 1. 608 1.583 

26.8 0.905 0.899 6l.2 2.130 2.068 

39.4 1.226 I.I24 69.3 2.824 2.746 

AMMONIUM Iridium CLORIDE (NH 4 ),IrCl e . 

SOLUBILITY IN WATER. (Archibald and Kern, 1917. 

Gms. (IS'n,) s JrCl 6 Gms. (NII,) 9 IrCl c 

}1 *' per 100 gms. H 4 0. t. per JOO gms. H 4 0. 

o.'2. o.556i 4o.o 1.5665 

10. o 0.7055 5o.o 1.9664 

i5.o 1.0910 60.0. 2.4567 

3o.o 1.1066 80.0 4-38i5 

Decomposition occurs at higher temperatures. 

SOLUBILITY IN AQUEOUS SOLUTIONS OP AMMONIUM CHLORIDE AT 20. 

(Archibald and Kern, 1917.) 

Gin. mols. Gms. (NH ) 2 IrCl, Gm. mols. Gms. (Nri,),IrCl fl 

IS'H CL per liter, per 100 gms. solvent. Nil, Cl por liter, per 100 gms solvent. 

o.io 0.1798 i.oo 0.0064 

O.20 0.0780 2.OO 0.0027 

IRIDIUM Anunoni urn CHLORIDE Ir(NHj Cl,, 

4 c. O 

SOLUBILITY OP IRIDIUM AMMONIUM CHLORIDE IN AQUEOUS 
SOLUTIONS op PLATINUM AMMONIUM CHLORIDB AND VICE VERSA AT 18. 

(Ogawa, 1930.) 
fin a. per 100 pas. sac. solution Ons. per 100 gws. sac. solution 

f K/V -* 



1.086 o.o 0.^24 0.364 

1.016 0.089 0.258 0.481 

0.902 0.196 0.197 0.594 

0.605 0.267 o.-ios 0.605 

0.524 0.288 0.0 0.768 



68i 



IRIDIUM Ir 



SOLUBILITY OF IRIDIUM AMMONIUM CHLORIDES IN tfATBR AT 19. 

(Deleplne, 1908.) 
Name of Salt. Formula. 

Ammonium iridium chloride (NH4)2lrCl6 0.77 

I>iammonium aquo penta chloro iridite IrClsCEkOXNH^ 15.4 
Triamrnonium hexa chloro iridite IrClt>(NH 4 )3+H 2 O 10.5 

Sodium CHLORIDE Irtta^Clg. 12H ? 

SOLUBILITY OF IRIDIUM SODIUM CHLORIDE IN WATER. 
(Ogawa, 19TO.) 



c o 


Ctas. ] 


[rNa ? ( 




_0 


Ins. IrNaj>Cl e 




r o 


fins. IrNaj>Cl 6 




per 100 


PIS. 


H 2 fc per 100 ana. H ? 


C 


per 


100 


gns. 


H * 


1 S - 


34 


.46 




40 


96.00 




63 




202 


.63 




&2. 


41 


-39 




4S 


123.96 




70 




231 


.66 




25 


t\(\ 


.11 




51 


155.26 




75 




253 


.17 




30 


56 


.17 




55 


169.27 




80 




279 


34 




35 


74 


03 




60 


191 .18 




85 




307 


.26 




JLRIDIUM 


DOUBLE 


SALTS. 


SOLUBILITY IN WATER. 


(Palmaer Ber. 23, 3817; 24, 2090, 


'91.) 












Double Salt. 


Formula. 






t 6 . 


Gms. 
Gms 


per TOO 
i.HaO. 


Irido 


Pentamine 


Bromide 




Ir(NH 8 )JBr 3 






12.5 




0. 


284 


" " Bromonitrate 


Ir(NH a ) 6 Br(NO 3 ) 3 


18 




5- 


58 


" " Tri Chloride LKNH^CU 


15.1 




6. 


53 


" *' Chloro Bromide 


Ir(NH 8 ) 5 ClBr 2 






15 




o. 


47 


** " Chloro Iodide IrfNHg^CHz 


J 5 




o. 


95 


" " Chloro Nitrate 


IrCNHJ^aCNOa) 


2 




i5-4 




I. 


94 


*' " Chloro Sulphate 


Ir(NH 8 ) 6 ClSO 4 .2H 2 O 


15.0 




o. 


74 








Nitrate 




Ir(NH 8 ) 5 (N0 3 ) 8 






16 




o. 


28 


" Aquo Pentamine Bromide 


Ir(NH 8 ) 6 (OH 2 )Br 3 


ord. temp. 


25- 







tt 


it 


Chloride 


Ir(NH 8 ) 6 (OH 2 )Cl 


3 


ord. temp. 


74- 


7 







K 


Nitrate Ir(NH 3 ) 6 (OH 2 ) (NOs) 8 




17 




IO. 


o 



SOLUBILITY OF EACH IN WATER AT 20 (Benrath, 1924.) 



Cl 



Compound. 

IVlono quinine hexa chlor iridate. 

brom 

K>i quinine chlor 

IVlono cinchonine 

o brom 

3L>i cinchonine chlor 

IVlono cinchonidine 

>> brom 

H)i cinchonidine chlor > 

Strychnine 

brom 

13 ru cine chlor 

> brom 

ISitron chlor 

brom 



Formula. 



(C 2 oH a< N a 2 ) s .H s IrCl u 



C 19 H aa N :1 O.H s IrBr li 

C 19 H as N 8 O.H 8 IrCl G 
C 19 H ss N s O.H s IrBr c 
(C tt HN > 0).HJpCl, s 

(C 91 H S3 N 3 9 ) 8 H s IrBr 6 



(C !1 oH llt N,).HJrBiv, 



Cms. cnipd. 
nor 100 cc. 

ir s o. 
0.0439 
0.0174 
0.0012 
c.1263 
o . 0062 
o.ooSy 
0.0277 
0.0048 
o . oo34 

<KOOl5 

o.oo83 
o.ooi5 
o . 0082 
0.0086 



Gms. niuls. 

cnipd. per lller 

sat. sul. 

6.0. 
1.7. 
I .2. IO- 5 

1.8.10-3 
6.5.10- 5 
3.5. io- 5 

3.9.10-* 

5.o. io- 5 
3.4.io- 5 
.1.3.10-* 

1.2. IO" 5 

7.0. io*" 5 

I .2. IO- 5 

8.0.IO- 5 



K KAL1UM 682 

IRIDIUM OXIDE IrO p .xH,,0 

One liter of water. sat. with Iririium Oxide contains 0.002 gm. j r Q 
at 20. ? 

One liter of 0.002 B IIC1 sat. wrif.li Iridium Oxide contains 0.0005 
gm. I0 p at 20. " (Hoser and Hachhofer, 1932.) 

POTASSIUM K ? 

SOLUBILITY OF POTASSIUM IN Liooin AMMONIA. 
Results of Ruff and Geisel, 1906 Results of Johnston and Meyer, 1929 

Moln. NH^ CO dissolve Q Qns. K dissolved 

1 1 &. aton K c per 100 gns. NH,, 

-100 4.8.2 -50.38 45.56 

"50 4.79 -33-5 46.38 

4.74 49-OS 

SOLUBILITY OF POTASSIUM IN MELTED KOH. (von Hevesy. 1909.) 
Difficulty was experienced due to the failure of the excess of K to separate com- 
pletely from the saturated solution. Time of heating, 50 hours. 
t. Cms. K per 100 Gms. KOH. 

480 7.8-8.9 

600 3 -4 

650 2 -2.7 

700 0.5-1-3 

Fusion-point data for mixtures of Potassium and Rubidium are given 
by Goria, 1935.) 



A10 POTASSIUM ALUMINATE K a Q.Al,0,.3lI 0. 

C. O G. 



ZT 

EQUILIBRIUM IN THB SYSTEM POTASSIUM HYDROXIDE, 
ALUMINUM HYOROXIDK AND VATRR AT 30. 

(Jucaitls, 1934.) 

The mixtures were shaken for 3 months. 



faa. per 1DO japs, sat, aol. Solirt Gtoa. per IQOjgns. sac, sol. Solid 

K.O ^3 Phase K^O Al 2?j Phase 

30.21 15.58 K 2 O.A1 .,0^.3^0 39.40 3-01 K 2 O.Al ? 3 .3l] ? 

30.87 12.51 " 41.25 2.20 " "* 

31.65 10.90 " 43-86 1.73 

32.03 9.79 " 44.74 1.26 " 

32.40 8.62 " 45-41 1.80 " 

35.67 4.68 " 46.06 1.25 

38.38 3.93 " 47.83 0.92 

POTASSIUM (Dihydrogen) ARSENATE KH 2 As0 4 . 

100 gms. sat. aq. solution contain 15.9 gms. KH 2 AsO 4 , or 100 gms. H 2 O dissolve 
r8;86 gms. at 6 . Sp. Gr. of solution = 1.1134. (Field, 1859.) 

loo cc. sat. aq. solution contain 28.24 gms. KH 2 AsO4 at about 7. 

(Muthmann and Kunlxe, 1894.) 

ioo gms. glyceroi (d u = 1.256) dissolve 50.1 gms. potassium arsenate at 15-16. 

(Ossendowski, 1907.) 



683 



KAL1UM K 



POTASSIUM ARSENITES K 4 As*0 7 , K 6 As 4 9 .iaH 2 0. 

EQUILIBRIUM IN THE SYSTEM POTASSIUM OXIDE, ARSENIC TRIOXIDE AND WATER 

AT 25. ( Schrcincmakors and Do Baat, 1920. ) 
For saturation 4 to 6 weeks agitation at 25 was employed. 

Gms. per ion gms. *'ii. ^>l. 
~As a (C 
48.^6 

44/84- 
39.49 
33. Go 
24.16 

'20.. 98 

2-2.47 
29.GI 

23.82 
17.57 
T i. 53 



Gms. per 100 gms. 


sat. sol. 


AS, o 3 !"~ fc ~"' " 


~"lt s 6r Solid Phase 


2. 02 


O.O ASgO-j 


22.63 


5.6l 


36. 29 


8.79 


41.93 


9- 6 9 




54.02 


11.62 




58.ii 


i3.;4 D 


.2 


53.49 


i5.24 




49-58 


17.28 




49.21 


18.61 




49.02 


20. 19 




49-47 


22. O I (?) 


49-65 


23 . 00 (?) 



o.o 



K,0. "" Solid I> 


liase. 


24^16 D :l . 


.12 


28.61 




23.49 




24.07 




28.05 




3*. 93 




35. 96 




38.32 




42.48 KOIl 


'HnO 


43.52 > 


> 


44.i3 KOH. 


2lI 2 O 



45.5 



AsO 



Di. 2 =K 2 As 4 0,= K 2 0(As a 3 ) :i , 



POTASSIUM BORAXES. 

SOLUBILITY OF POTASSIUM BORATES IN WATER AT 30. 

(Dukelski Z. anorg. Chem. 50, 42, '06, complete references given.) 



Gms. per TOO Gms. Solution. Gms. per loojCrms. Residue. 

* 



K 2 O. 


B 2 3 . 


K 2 O. 


B 2 3 . ' 


47-50 








46.36 


0.91 


46.13 


9.02 


40.51 


1.25 


41 .62 


9.71 


36.82 


i. 80 


39-90 




3 2 -74 


3 .51 


37-22 


14.58 


29.63 


6.98 


35-05 


17.92 


24-84 


17-63 


30.02 


21.70 


23-3 


18.19 


26.84 


31-49 


16.21 


13.10 


25.12 


33-18 


11.78 


9.82 


20.57 


26.43 


9.18 


8.00 


22.38 


3 T -3 


6.22 


9.13 


20.87 


31.06 


7-73 


13-37 


22.21 


36.24 


7.81 


13.28 


17.50 


34-18 


7.71 


13.21 


11-49 


34-81 


7-63 


13.28 


12.51 


40.52 


3-42 


7-59 


10.77 


37-35 


i. 80 


4.15 


5 .88 


20-00 


0.51 


3.19 


I0.8l 


40.89 


0-33 


4-58 


7.72 


34-21 


0.31 


4.46 


3-9 1 


30.68 




3-54 







Solid 
Phase. 

KOH.2H 2 O 



BO 



K 2 0.2B 2 O 3 .4H 2 O + K 2 O.5 



K 2 O.5B 2 3 .8H 2 O 



K 2 0.sB 2 O 3 .8H 2 O4- B(OH) a 



POTASSIUM MetaBORATE KB0 2 . 

Fusion-point data for potassium inelaborate + sodiuni metaborate and for 
potassium metaborate + potassium metaphosphate are given by van Klooster 
(1910-11). 



K KALI DM 68 4 

POTASSIUM PerBORATES, 2KB0 3 .H 2 O, 2KB0 3 .H 2 2 . 
SOLUBILITY OF EACH IN WATER. 

(v. Girsewald and Wolokitm, 1909.) 



Borate. 


% Active O in f Cms. Salt per too 
Botate. * Gms. Water. 


2KB0 3 .H 2 


14-93 


o 


1.25 


2KB0 3 .H 2 Q2 


14.93 
20.84 


IS 
IS 


2.50 
0.70 


POTASSIUM Di BORATE K 


: p p.aB p 8 .5 


or 6 H 2 





looocc sat. solution of Potassium Diborate in Water has a normality 
of 0.9 with respect to K at o. A similar solution saturated with 
potassium pentaborate has a normality of 0.07 with respect to K. 
(Rosenheim and Leyser, 1921.) 

POTASSIUM Penta BORATE K 2 0.sB ? 3 .8H 2 

SOLUBILITY op POTASSIUM PENTA BORATB IK WATER. 

(Bullet and Andres, 1970.) 

The pentaborate was prepared by the action of boric acid upon potas- 
sium chloride and upon potassium nitrate at temperatures above 100 in 
presence of water vapor. The anhydrous salt hydrates easily in moist 
air. 



o (?ms. KpO.SBj^), Solid 
per 100 0ns. sac. sol. Phase 


t O ftns. K ? 0. fiB ? 0.j Solid 
per 100 gws. sat. sol. Phase 


-o.53(Eu 


tec) 1.54(1.50) ICP+ KgO.sBpGUtf 







1.56 K ? .5B 2 3 .8H P 


76.65 13-62 


5 


1.77 " "' 


82.3 15-5 




18 


2.66(2.75) " 


87.15 17.02 ' 




25 


~ (3.41) 


89.8 18.00 




30 


3.8 


94.8 19.85 




45 


5-72 


100 22.3 ' 


57.6 


8.45 


ioi-.65 23.0 " 


62.8 


9.8s 


i02.3(b.pt.) 23.4 " 


69.0 


11.5 





The authors also found that at about 170 the solid phase is trans- 
formed to KJD.5B ? 3 .2H ? and above 350 it becomes the anhydrous com- 
pound which melts at 780 * 

The values in parentheses in the above table are by Menzel, 1937.) 

EQUILIBRIUM IN THE SYSTEM POTASSIUM TETRABORATK, POTASSIUM PENTABORATE 
POTASSIUM CHLORIDE AND WATER AT 35. 
(Teeple, 19 ?g.) 

Solid 
Phase 

KCI 



ioi6* 
KCI * K ? B %flV* 

KCI * K,B 10 lfl .8H p O 
K B 4 7 .iiH;8 i K 8 B; O^. 
KCI t- " + " 





Gtas. per 100 go 


is. K?0 


' KCI 




VioV 


39-0 











21.3 











5.0 


37.3 


5-9 





38.1 





3-0 





23.8 


8.0 


36.8 


6.7 


3.5 



POTASSIUM 



Fluo BORATE KP 4 B 



685 



KALJUM K 



One liter of water sat. vdth Potassium fluoborate at room temperature 
(20?) contains 0.04.5 m mols. KF B. (deBoer and van Liempt, 1927.) 

100 gins. H p O dissolve 0.44. gm. KF B at 20 and 6.27 ?ms. at 100. 
(Stolba, 1889.) 



EQUILIBRIUM IN THB SYSTEM POTASSIUM FLUOBORATE, 
POTASSIUM PBRCHLORATF, AND WATBR AT 25. 

(Ray and MUra, 1934.) 



Oms. per IPO gas, sat, sol. 



0.574 
0.562 
0.569 
0.589 
0.588 
0.558 
0.476 
0.1*33 



KC10 4 


1 Phase 


0.0 


KF.B 


0.213 


it 


0.276 


H 


0.328 


it 


0.393 
0.432 


"+8KF.B.KC10. 
8FCF 4 B.KC10 4 


0-549 


11 


0.684 


ti 



Oms. per 100 


0ns. sat. sol 


Solid 


' KF 4 B 


KC10 4 


1 Phase 


0.420 


0.814 


8KF 4 B.KC10 4 


0.427 


0.943 


H 


0.437 


1.012 


11 + 2fCF B.KI 


0.4.06 


1.077 


2 KF 4 B.Kil0 4 


0.385 


1.165 


n 


0-337 


1-433 


M 


0.243 


1.6l6 


KC10 4 


0.0 


1-971 


" 



EQUILIBRIUM IK THE SYSTEM POTASSIUM FLUOBORATB 



POTASSIUM PERIODATB AND WATBP AT 

(Ray and Mltra, 1935.) 



35 U 



The results are given only in the form of a triangular diagram from 
which the following approximate values were read. 



flms. per 100 gns. sac. sol. 
/ KF70 KIO. 



Solid 
Phase 



Qns. per 100 gna. sat, sol. 

' KF.B KIoT y 

' 



Solid 
Phase 



0.92 
0.91 
0.90 
0.80 



0.0 
0.2 
0.4. 
0.4.2 



KF 4 B 



KI0 4 



KIO. 



0.60 
0.40 
0.20 
oo 



0.48 
0.55 
0.68 
0.80 



EQUILIBRIUM IN THE SYSTEM POTASSIUM FLUOBORATB 
POTASSIUM PERMANGANATE AND WATER AT 25. 

(Ray and Chaturji, 1932.) 



KT0 



Qms. per 100 & 


ijs. sat. 


sol. Solid 


f KF 4 B 


KMn0 4 


^ Phase 


0.57 


0.0 


KF 4 B 


0.54 


1.12 




0.46 


1.58 


n 


0.22 

0.41 


2-07 
3.19 


" 4 KF,B.6KMnO, 
KF B.6Kn0 4 


0.50 


4.08 


n 



Qua, per 100 g%s. sat, sol. 



0.48 

0.37 
0.22 
0.33 
0.28 
0.0 



42 
03 
32 

76 

90 



Solid 
Phase 



KMnO. 



KMnO. 



POTASSIUM BKOMIDE KBr. 

FREEZING-POINTS OF AQUEOUS SOLUTIONS OF POTASSIUM BROMIDE. 
(Klein and Svanborg, 1920; Rodebush, 1918.) 



Gms. KBr per 
loo ft 1 , sat. sol. 



t". 



Cms. KBr per 
100 gms. H 2 0. 



.348. 
.863. 
,694. 



1.19 fK and Si 3.19 11.53 

2.975 5.6i 20.42 

5. 9 5 >, 6.57 23.82 

8.5i 30.87 



-10.55 

10.90 

19. ,6Euieo. . . 



Cms. KUr per 
100 gins. 1LO. 

. 38.33 
. 3g. 5o 
45.65 



K KALIUM 

POTASSIUM KBr, 

SOLUBILITY IN WATER. 

(Average curve from results of Meusser Z. anorg. Chem. 44, 70, '05- 

'84; Ann. chim. phys. M 2, 526, '94; de Coppet Ibid. [5] 3 

Sfienstone Phil. Trans. 175, 23, '84. 



Etard Compt. rend. 08. 
3<V*i6, '83; Tilden and 



- 6.5 

- 8 -5 
-10.5 

-ii. S 

- 5 
o 

5 
10 

15 

20 

2 5 



Grams KBr per TOO Grams 



Solution. 
20-0 
26.5 

29-5 
31.2 
31-8 

33-3 
34-9 



37 
38 
39 



40.4 



Water. 
25.0 

35-7 
41-8 

45-3 
46.7 
50.0 

53' 
56- 

59- 
62. 

65- 



67-7 



5. 275* 23. 

t. 


Grams KBr per 


ioo Grams 




Solution. 


Water. * 


30 


41.4 


70.6 


40 


43 -o 


75-5 


50 


44-5 


80.2 


60 


46.1 


85-5 


70 


47-4 


90.0 


80 


48.7 


95-o 


90 


49-8 


99.2 


100 


51.0 


104.0 


no 


52-3 


109.5 


140 


54-7 


120.9 


181 


59 -3 


145 - 6 



of the Soiubiiity f 



a or Qms 


. KBr per 


o 


d of Qua. KBr oer 




sat. sol. 


100 gi 


ns. sac. sol. 


t w 


sat. sol. 


100 0r 


IS. 81 


at. sol 


12. 




5<Eutec) 
1-3237 


31 
35 


.27 
.08 


(3) 


35 
50 


1-3941 


42.58 

44. 8; 


<3) 
(l) 


15 
20 


1 

i 


3597 
3701 


38 
39 


-59 
-73 


(3) 
(2) 


50.21 

75 


1.4l6o 


44 

48 


.95 
.3 


(3) 
(l ) 


25 
25 

25 


l 
l 
l 


3790 
3794 
3794 


40 
40 
40 


.65 
.71 
-57 


(l) 
(2) 
<4) 


91-95 
100 
100 


1-4590 
1.465 


50 
5i 


.36 

.2 


(3) 
(1) 
(5> 



i \ l l Ilerln? '; 1 9 3 6 > <a) Flottmann, 1928; (3) Scott and Durham, i 930 : 
(4) Scott and Prazier, 1927 ; (5) BrSnsted, 1913. J 

The following values for the solubility of Potassium Bromide in water 
at temperatures above 100, determined by the synthetic method are given 
by Benrath, Gjedebo, Schiffers and Vunderlich, 1937 ' 



c 


Gtes. KBr per 


c 


Gtas. KBr per 


t o 


Qns. KBr per 




100 0ns. sac. sol. 




100 3A8. sac. sol. 




100 9QS. sac. sol. 


103 
167 

208 


51-5 
57.5 
6l.l 


232 
251 
275 


63.1 
6 5 .2 
66.7 


301 
359 

'|21 


67.7 
70.7 
73-3 



SoLTJBtLITY OF MIXTURES OF POTASSIUM BROMIDE AND SlLVER BROMIDE IN WATER 

(Lambert, 1926.) 
The mixtures .were constantly stirred in a thermostat. 



Gms. per .100 gms. sat. sol. 

^ "*"^^ S^ ^aiull"" ' ' -^ O..l!l 


Gms. per 1 00 gms. sat. sol. 




AgBr. 


kMUlU 

KBr. Phase. 


t. 


* e ** afc - 
AgBr. 


s^^av ~ 
KBr. 


Solid 
Phase. 


-4-3o 
4o.... 


1.67 

1.636 
a. 24 


39-87 AgBr-hKBr 
39.54 
4o.88 


70... 
70... 
80... 


. 5.80 
. . 5.60 

6.72 


45.48 

45.53 
46.91 


AgBr+KBr 


60.'..".' 


3.' la 
4.20 


43.09 
42.43 
44.24 


90... 
ioo. . . 


- 8.47 

<).00 

. 10.55 


48.i5 
47.98 
48.66 


>} 



KAL1UM K 



SOLUBILITY OF POTASSIUM BROMIDE IN BROMINE WATER AT 32. 

(Joseph, 1920.) 

The mixtures were constantly agitated in a thermostat for 24. hours. 



Gms. per 100 gms. H S 



(I Of 


- ""vetoes 


V^SP**" 


sal. sol. 


Br. 


KBr. 


K3C)I7 


O.O 


72.56 


i.4o63 


'1 . 40 


7 3.3 9 


i . 4070 


3.21 


73.82 


i. 4 1 3 2 


3.96 


74.07 


1.4356 


7.43 


7>5 . 02 


1.4633 


12.09 


76.43 



Onis. per JOO gins. I 



'/Of 


' *um***^,-~ 


* ^aaMB" ~ 


sal. sol. 


lir. 


KBr. 


1.4753 


13.72 


77. I [ 


i . 5 236 


22.97 


80. i3 


1.5980 


38.21 


84.^9 


v. . 5 96 


/{3o.4 


210.4* 


2.860 


1472.0 


279.6* 



* In these two cases the mixtures were simply left in bottles for some days at about 28, and 
the heavv dark liquid filtered through glass wool and analyzed. The densities were taken by 
means of a Westphal balance. 



SOLUBILITY OP POTASSIUM BKOMOB IN AQUEOUS SOLUTIONS 
OF HYDROBROMIC ACID AT 25. 

(Scott and Durham, 1330.) 
cms. per 100 gms sat. solution 



HBr 
0.0 

6.88 
13.23 
18.07 



KBr 

140.62 
30.99 
22.69 
17.60 



Br 



SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM BROMATE AND VICE VERSA. 

(Ouerassimow, 1934.) 



Qms. per 100 
gms. sat. sol. 



Results at o 



Solid 
Phase 



Oms. per 100 
0ns. sat. sol. 



Solid 
Phase 




Solid 
Phase 



Results at 40 icon.) Results at 60 (con.) 



35-3" 


0.0 


KBr 


42.44 


i 


.28 


KBr 


10 


.07 


12 


.74 


KBrO, 


35.08 


0.57 


11 


42.34 


2 


.19 


" -4- 


KBr0 3 9 


52 


12 


.83 






o.6s 


" + KM> 3 


35-97 


2 


.60 


KBrO 


3 9 


37 


13 


. 14 


M 


0.0 


2.96 


KRrO z 


20.84 


4 


32 


" 


4 


.48 


14 


.92 


" 


Results 


at 20 





8.50 
o.o 


7 
11 


.32 

.70 


.. 


4 
3 


.35 

.94 


15 
16 


.58 

43 


t> 


39-4" 


0.0 


KBr 













.0 


18 


.21 


n 


39.26 


1.22 


" + KBrO 


Results at 60 















22.20 


1.85 


KBr0 3 


Results 


at 80 


11.80 


2.73 


it 


46.2 





.0 


KBr 












0.0 


6.43 


< 


45. 17 


3 


.70 


" * 


KBr0 3 49 


.72 





.0 


KBr 


Results 


at 40 





49.93 
44.56 


3 
3 


.75 
.73 


KBrO 


3 46 
45 


.5 

-57 


5 
5 


.62 
.60 


" -4- KBrO^ 
KBr0 3 3 


43-54 


0.0 


KBr 


31.90 


5 


.71 


" 


7 


.45 


20 


74 


11 


42.97 


0.34 


" 


12.69 


12 


.09 


" o.o 


25 


.53 


" 



K KAL1UM 688 

SOLUBILITY OP POTASSIUM RROMTDE IN AQUEOUS SOLUTIONS 
OP POTASSIUM BROMATB AND VICR VERSA AT 25 . 

(RlCCl. 1334.) 

Solid 
Phase 

KBr 



d of 


Ores, per luO 


pis. sac. sol. 


sac. sol. 


' KBr 


fCBrO ? \ 


1.381 


40.02 


O.O 


1.389 


^0.08 


1 .20 


1-392 


40.00 


1-43 


1.328 


34.82 


1.62 


1.237 


26.05 


2.06 


1. 161 


17.48 


2.73 


1.089 


7.82 


4.29 


1.054 


0.0 


7.533 



" + KBrO 
KBr0 3 



SOLUBILITY OP POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM CHLORIDE, AND OF POTASSIUM CHLORIDE IN AQUEOUS 
SOLUTIONS OF POTASSIUM BROMIDE, AT 25.2. 

(Touren Compt. rend. 130, 1252, 'oo.) 

KBr in Aq. KCl Solutions. KCl in Aq. KBr Solutions. 

ft 

Br 



Mols. per Liter. 


Grams per Liter. 


Mols. per 


Liter. 


Grams per Liter. 


KCl. 


KBf. 


KCl. 


KBr. 




KBr. 


KCl. 


Klir. 


KCl. 


0.0 


4.761 


O.O 


567.0 




O.O 


4-l8 




o 


.00 311 


.8 


0.67 


4-22 


5O.O 


502.5 




0-49 


3 -85 




58 


4 


287 


.2 


0.81 


4-15 


60.4 


494-2 




0.85 


3-58 


101 


3 


267 , 


.1 


I -35 


3-70 


100-7 


440.7 




I .31 


3-19 


IS^ 


.1 


238 


.0 


1.48 


3-54 


110.4 


421 .6 




1.78 


2 .91 


211 


9 


217- 


.1 


1.61 


3-42 


120.0 


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 


I83-5 


297.7 


















3-775 


o-5 2 S 


281.6 


62 5-3 


















SOLUBILITY- op POTASSIUM BROMIDE IN 


AQUEOUS SOLUTION OP POTASSIUM 






CHLORT.DE 


AND VICE 


^ERSA AT 


25. 












(Foe A, 1897.) 


Grams per Liter 
Solution. 


Milligram Mols, 
per Liter. 


"few 


ent Sp.Gr.of 


Mol. per cent 
KCl in 


KBr. 


KG". 


KBr. 


Ml 




Solution 


Solid 


Phase. 




558-I 


o.oo 


4686.2 


o. 


o 


0-0 


I 


3756 







.00 




531-5 


23-44 


4462.7 


3*4- 


2 


6.16 


I 


3700 







OO 




503.6 


46.57 


4228.5 


624. 


3 


12.86 


I 


.3648 




8 


23 




454-6 


82.62 


38I7-8 


1108. 





22.49 


I 


3544 




15 


.68 




379-6 


136.6 


3I88.I 


1830. 


7 


36.48 


I 


3320 




33 


.66 




324-8 


166.9 


2727.6 


2237. 


4 


45.06 


I 


3 TI 9 




63 


'5 1 




2.18.0 


213.9 


1830.2 


2868. 


b 


60.30 


I 


.2689 




82 


.29 




140.7 


250.9 


IlSl.I 


3363- 


9 


74.01 


I 


2 455 




88 


-04 




47-5 


291.7 


398.8 




4 


85.22 


I 


.1977 




96 


. 9 8 




O.O 


3 XI -3 


O-O 


4173- 


i 


100.00 


I 


.1756 


IOO 


00 





689 KAL1UM K 

SOLUBILITY OF POTASSIUM BROMIDE AT 25 IN: 

Aq. Solutions of KC1 and Vice Versa. Aq. Solutions of KI and Vice Versa. 

(Amadori and Pampanini, 1911.) (Amadori and Pampanini, 1911.) 

Cms, per 100 Cms. H g O. Cms, per 100 Cms. H 2 O. 

KBr. KCT ""KBr^ " KlT 

68.47 o 53.21 35.92 

62.26 5.43 42.32 66.63 

58.50 8.46 34.14 95.36 

52.45 12.48 30.08 H9.52 

45.42 17.17 29.62 119 

38.70 21.23 22.15 127.10 

26.62 25.88 21.88 127.31 

12.94 31.02 18.54 130.61 

o 36.12 o 149.26 

SOLUBILITY OP MIXTURES OP POTASSIUM BROMIDE AND CHLORIDE AND 
OF MIXTURES OF POTASSIUM BROMIDE AND IODIDE IN WATER. 

(Etard Ann. chim. pbys. [7] 3, 275, '97.) 

Mixtures of KBr and KC1. Mixtures of KBr and KI. 

t Prams per TOO Cms. Solution* Grams per 100 Grams Solution. 

. . _ , , _- _ > 

-20 17.5 10.5 9-2 42.5 

o 21.5 10.8 9.9 45-3 Br 

IO 23.2 II. O 10.2 46.6 

20 24.8 1 1. 2 10.5 47-5 

25 25.5 II-3 10-7 48.0 

30 26.3 II.4 10-9 48.6 

40 28 . o 1 1 . 5 ii .2 49 . 6 

60 30.6 n. 8 ii. 9 51.3 

80 33.4 12. i 12.6 52.7 

100 35.. 7 12.6 13.2 53.8 

I2O 38.0 12-9 14.0 54.8 

150 40.6 13.4 14.9 55.5 

Data for the reciprocal Salt pair 

(KBr) j, MgCl z (KC1) 4 MgBr ? 

recalculated from the results of Boelce, 1908, and others are given 
by JStoecke, 1938. 

SOLUBILITY OF POTASSIUM BROMIDI IN AQUBOUS SOLUTIONS op 
POTASSIUM CHLORATE AND VICE VERSA AT 25. 

(FUcci. 1937.) 

6 of Qs. p*r loo ffaa. sac. sol. Solid 

aat. sol. ' K3r KCIO^ ^ Phase 

380 40.63 o.o KBr 

356 40.02 1.42 " t KC10 3 

376 39*47 1.42 KC10 3 

292 31-66 1.87 " 

216 24.20 2.41 " 

160 16.99 3.21 " 

1.100 9-30 4.59 " 

1.047 o.o 7.905 " 



K KALIUH 



Br 



690 
SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 



<i or 
sac. SOL 



POTASSIUM IODATB AND VICE VERSA AT 

(Riccl, 1934.) 



Qns. per 100 gins. sat. .sol. 

1 K3T KlbT N 
3 



25 AND 50 



Results at -5 



1-333 
1.352 


36.25 
35.71 


0.0 

1.80 


1.290 
1.208 


30.50 

22 o9 


1.7-7 
1.80 


1 .136 
1.080 
1.043 


14.80 
7.58 
0.0 


1.95 

2.45 
5.186 


Results at 25 


1.381 
1.396 
1.407 
1.341 


40.62 
40.28 

39.75 
34.38 


0.0 
0.98 
2.36 
2.47 


1.294 


25.91 


2.73 



Kttr 



KI0 



Solid 
Phase 


d of Oms. per 100 gyas. sat. sol. J 


sat. sol. ' KBr 


KI0 3 x F 




Results at 25 


(con. ) 


+ KI0 3 


1.168 17.40 
1.106 8.35 
1.071 o.o 


3.26 KTO ? 
4.53 
8.452 " 



Solid 
Phase 



KBr 



+ KIO, 



KIO 



Results at 50 

44.77 
43-88 
43-50 
38.03 
30.57 
23.19 
15.65 
8.18 

0.0 



0.0 
2.22 
3-07 
3.32 

3-87 
4.66 
5- 



KBr 



KIO, 



KI0 



.80 
8.16 

1 3 . 20 " 

SOLUBILITY OP POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM NITRATE, AND OP POTASSIUM NITRATE IN AQUEOUS 
SOLUTIONS OF POTASSIUM BROMIDE, AT 14.5 AND AT 25.2. 

(Touren Compt. rend. 130, 908, 'oo.) 

KBr in Aqueous KNO 3 Solutions. 

Mois. per Liter. Grams per Liter. 



KNO 3 in Aq. KBr Solutions. 

Mols. per Liter. Grams per Liter. 



KNO 3 . 


KBr. 


KN0 3 . 


KBr 




KBr. 


KN0 3 . 


KBr. 


KNO 3 . 


Results at 14. 


2. 


Results at 14.20. 


O-O 


4 


332 








5*5- 


9 


o.o 


2 .228 


O 


.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 


1-835 


93 


4 


185.7 


1-235 


3 


939 


124 


-9 


469. 


I 


I -092 


1-730 


130 


.0 


*75- 
















1-577 


1.587 


187 


.8 


160.6 


Results t 


it 25 


.2. 










2.542 


I .406 


302 


7 


142.2 


0-0 


4 


.76l 


o 


-O 


566. 


2 


3-S36 


1.308 


421 


.i 


132-3 


O.I3I 


4 


.72 


J 3 


3 


561. 





Results at 25.2. 


0.527 


4 


-6l 


53 


3 


549- 


I 


0-0 


3.217 


o 


.0 


325-5 


0.721 


4 


54 


72 


9 


540. 


8 


0.38 


3.026 


45 


3 


306.2 


1.0 9 


4 


475 


110.3 


533- 


o 


o-93 


2.689 


no 


.8 


272 .0 


I .170 


4 


44 


us v 


4 


528- 


8 


I -37 


2.492 


163 


.1 


252 .2 


1.504 


4 


375 


*52 


.2 


521- 


i 


I. 208 


2 -2l6 


143 


.8 


224.3 
















2.87 


1.9 5 8 


341 


.8* 


igS.I 
















3-55 


1.807 


422 


.8 


182.8 



SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM HYDROXIDE. 

(Ditto Compt. rend. 124, 30, '97.) 



Grams per TOOO Grams HoQ. 

' KOH. ' KBr. ^ 

36.4 558.4 

II3-5 433-6 

177-2 358.1 

231.1 281.2 



Grams per 1000 Grams Hi>O. 



KOH. 
277.6 

434-7 
579-6 
806.9 



KBr. 
248.1 

I37.I 
64-8 

33-4 



691 KAUUM K 

SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM HYDROXIDE AT 20. (Bronsted, 1920 a.) 

J^^l!s^^ ^^^^^' V ^L^^~~^ Gm. mols. pei* liter. 

KOII. KBr. ""~R QJT*~*~*^i]lr. ^ 

12.19 0.348 14.02 0.246 

12.92 o.3o6 i4.85 0.214 

i3.84 0.247 10.02 0.210 



SOLUBILITY OP MIXTURES OF POTASSIUM BROMIDE AND AMMONIUM 
BROMIDE IN WATER AT 25. 

(Fock Z. Kryst. Min. 28, 357, '97.) 




Grams per Liter Solution. 


Mol. per cent in Solution. Sp. Gr. of 


Mol. per cent 


in Solid Phase. 


NH 4 Br. 


KBr. 


NH 4 Br. 


KBr. 


Solutions. 


NH 4 Br. 


KBr. 


o.oo 


SS8.I 


0-0 


IOO 


^3756 


o.oo 


IOO 


6. 4 


554-2 


I. 3 8 


98.62 


1-3745 


0.26 


99-74 


24.64 


536.5 


5- 2 9 


94-71 


1-3733 


1.27 


9^-73 


5^-34 


516.8 


10.77 


89.23 


1.3721 


3-02 


96.98 


152.9 


441.2 


29.63 


70-37 


1.3711 


8.42 


91.58 


262 .2 


347-3 


47 - 8 4 


52.16 


1-37I5 


17.20 


82.80 


347-6 


262.3 


61 .69 




J-3753 


27.98 


72 .02 


381.4 


260.3 


64.03 


35-97 


I -3753 


32-53 


67.47 


417-8 


232.2 


68. 61 


31-39 


1.3766 


39-45 


60-55 


432-5 


222.3 


70.27 


29-73 


1-3777 


variable 


variable 


480.8 


179.9 


76.47 


2 3 -53 


1.3766 


9 8 -53 


i-47 


577-3 


o .0 


100.0 


0.0 


i . 7763 


IOO-O 


o .00 



Br 



SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS 
OP METHYL ALCOHOL AT 25. 

(Akerlof and Turck, 1935.) 

ftas. CHjjOH per Ore. Mols. KBr Onus. CHjOH per Gta. Mols. KBr 

100 gms. solvent per 1000 gms. 100 gms. solvent per 1000 gas. 

mixture solvent mixture mixture solvent mixture 

o.o 5.784 80.03 0.^625 

20.0 3-711 89.79 0.2629 

40.82 2.l8o 94.76 0.2049 

59.56 1.182 100.0 0.1805 

72.39 0.7697 

SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF 

ETHYL ALCOHOL AND OF METHYL ALCOHOL. ( Zoitlin, 1026. ) 

The mixtures were agitated frequently by hand during 5 days. The temperatures 
remained constant to i. 

Results for Methyl Alcohol. Results for Ethyl Alcohol. 

Gm. mols. K Br per liter at Gm. mols. K Drper U tor at 

CII 3 OH in solvent. J0".:>. 19,9. C 2 II 5 OH in solvent. 10V>. aO.9. 

25.96 2.4?5 2.49^ 25.07. 2.3-27 2.437 

45.i3 1.426 1.466 5o.oi i. 01 6 1.161 

74.88 0.411 0.434 7-5. o3 0.2704 o.2cj55 

100.00 o.i37(> o.ijjtt 97 -3 - o.oii.f 

100 gms. aq. 5o wt. % ethyl alcohol dissolve 16.4 gnis. K Br at 20. 

(\YrigU, 19-16.) 



K KALIUM 692 

SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF METHYL 
ALCOHOL AT 25. 

(Here and Anders, 1907.) 

Wt.%CH*OH Gins. Or per , ftf c- t c^i Wt. % CH a OH Cms. Or per , f <,. ~, 

insolvent. 100 cc. Sat. Sol. ^ of Sat. SoL insolvent. zoo cc. Sat. Sol. ^ of Sat. Sd. 

o 56.04 1-3797 64 10.35 0.9801 
10.6 46.28 1.300 78.1 5.24 0.8906 

30.8 29.98 I-I59 98.9 2.74 0.8411 

47.1 19.28 1.058 loo 1.69 0.8047 

The solubility of potassium bromide in methyl alcohol at the critical tem- 
perature is given by Centnerszner (1910), as 0.2 gm. KBr per 100 gms. sat solution. 



SOLUBILITY OF POTASSIUM BROMIDE IN DILUTE AQUEOUS ETHYL ALCOHOL. 



Br 



Results at o. 
(Armstrong and Eyre, 1910-11.) 


Results at 25. 
(Armstrong, Eyre, Hussey and Paddison, 1907.) 


Wt. % CsH 6 OH 
in Solvent. 



Gms. KBr per 
too Gms. Sat. Sol. 

34-92 


Wt. % QHjOH 
in Solvent. 
O 


Gms. KBr per 
loo Gms. Sat. Sol. 
40.78 


</ of Sat. Sol. 
'1.3824 


I.I4 
2.25 
4.41 
8.44 


34-35 
32.96 
31-99 
29-43 


1. 14 
2.25 

4.41 
12.14 

18.73 


39.54 
38.41 
34-97 
30.91 


1.3727 
1.3634 
1-3443 
1.2815 
1.2322 



THE SYSTEM POTASSIUM BROMIDE, TERTIARY BUTYL 

ALCOHOL AND WATER AT 30. 

(Olnnings and ftobbina, 1030.) 

The points on the Dinodal curve of this system were determined by 
observing the appearance or disappearance in a mixture of weighed 
amounts of the other. Conjugated points were 

The points on the bi nodal curve of this system were determined by 
observing the appearance or disappearance of clouding in a mixture of 
weighed amounts of KBr and one of the liquids, upon addition of a 
weighed amount of the other. Conjugated points were found by deter- 
mination of KBr in two liquid phases in contact with each other and 
from these the plait point (p.p.) was obtained by plotting. 



oms. 


per 100 




Ons. per 100 


Oms. 


per 100 


1ms. 


per 1QO 




gms. 


mix cure 




gns. mixture 





as. 


mixture 




8 


P18. 


mixture 




'(CH,) 3 COU KBr" 


IcH^jCOH KBr' 'i 


fCH^) 3 CQh KBr x A (CH 3 ) 3 C01 


H K3l 


* N 


70.2 


3- 


i 


50.3 6.7 


27 


.7 


12 


.6 


11 


.3 


22. 


6 


tf5.7 


4 


2 


44-7 7.8 


25 


.6 


13 


4 


9 


. 2 


25. 


3 


60.7 


4. 


8 


42.0 8.7P-P- 


20 


.0 


15 


.7 


7 


.7 


28. 


5 


56.9 


5- 


4 


35.7 10.0 


17 


.0 


17 


.O 


6 


.8 


30. 


4 


53.4 


6. 


1 


29.7 11-9 


13 


.4 


19 


.8 


6 


. i 


33. 


1 



693 KALIUM K 

SOLUBILITY OF POTASSIUM BROMIDE IN AQUEOUS ALCOHOL. 

(Taylor J. Physic. Ch. i, 724, 'g 



Results at 30. 

Gms. KBr per TOO Gms. 


Sat. Solution. 


Solvent. 


41 .62 


7I-30 


38.98 


67.25 


36.33 


63.40 


31.09 


56.40 


25.98 


50.15 


21 .24 


44-95 


16.27 


38-85 


11.50 


32.50 


6.90 


24.70 


39 


15-95 


0.87 


8.80 



Results at 40. 

Cms. KBr per too Gms. 



Wt. per cent Alcohol 
in Solution. 

O 

5 
10 

20 

30 
40 

50 
60 
70 
80 
90 

SOLUBILITY o? POTASSIUM BROMIDE AT 25 IN: 

(Herz and Knoch, 1905.) 



Sat. Solution. 


Solvent. 


43-40 


76.65 


40.85 


72.70 


38.37 


69.00 


33-27 


62.30 


28.32 


5 6 -45 


23.22 


50-46 


i8.ii 


44-25 


13.02 


37-40 


7.98 


28.90 


3-65 


18.95 


1.03 


10.45 



Aqueous Acetone, 
cc. Acetone ^ er 10 cc> Sat. Solution. 


Sp. Gr. 
Solutions. 


wt. % 

Glycerol 
in Solvent. 


Aqueous Glycerol 
KBr per 100 cc. Sol. 


Sp. Gr. 
Solutions. 


per ioo cc. Millimols 
Solvent. KBr. 


Gms. 
KBr. 


Gms. 
HjO. 


Millimols. 


Gms. 





4 8l. 


3 


57-3 


80.6 


I 


3793 


O 


481. 


3 


57-32 


1-3793 


20 


366, 


7 




69.5 


I 


.2688 


I3-28 


444- 


3 


52.91 


1.3704 


30 


310. 


-5 


36*98 


62.97 


I 


.2118 


25.98 


404 




48.11 


1.3655 


40 


259 




30.85 


55.60 


I 


.1558 


45.36 


340. 


5 


40.55 


1.3594 


50 


2O2. 


9 


24. 16 


47-6o 


I. 


.0918 


54.23 


310. 


4 


36.98 


1.3580 


60 


144. 


9 


17.22 


39-15 


I. 


.0275 


83-84 


219. 


25 


26.11 


1.3603 


70 


95-3 


n-35 


29.78 


O. 


9591 


IOO 


172. 


65 


20.56 


1.3691 


80 


4 6. 


5 


5-54 


2O. IO 


0. 


,8942 












90 


IO. 


i 


i. 20 


10.15 


0. 


8340 













3r 



xoo gm. acetone dissolve 0.023 S** 1 - KBr at 25. 

(Krug and McElroy J. anal. Chem.tS, 184, 'pa.) 

ioo gms. Glycerol of d'= i.23-26(= 86.5 /o) dissolve 20.69 gms. K Br at 20. 
d 1.2645(= Q8.5 /o) i?.i5 

(Holm, 1921, 1922.) 

ioo cc. sat .solution of potassium bromide in ethyl urcthan (m. pt. 4*9-6) contain 
0,387 gms. K Br at 60. (Siuckgold, m?.) 



THE SYSTEM POTASSIUM HROMIDB ETHYLENE GLYCOL 
AND WATER AT 30. 

(Trimble. 1931.) 



d of 
sac. solution 

1.3876 
1*3417 
1.2995 
1.2637 
1,2338 
1.2131 



Gtaa. per 100 0ms x sat. solution 



'KBr 


CH ? OHCH^OH 


H ? * 


41. 58 


0.0 


58.42 


35.32 


12.73 


51-45 


29.64 


28.29 


42.07 


23.58 


46.08 


30.34 


18.03 


65.67 


l6,30 


13.68 


86.32 


0.0 



K KALIUM 694 



SOLUBILITY OF POTASSIUM BROMIDE IN AMUROUS SOLUTIONS OF DTOXANE AT 25. 

(her?, and Lorentz, 19?9.) 

cc Dioxani Gsn.. Mol. K3r Qms. KBr per 

per !CX)cc solvent per liter sat. sol. liter sat. solution 

10 4,20 500 

20 3 -70 44O 

33 2 - f > 345 

Two liquid Layers are formed between 47 and 85 vol. percent Dioxane. 
The lower contains 2.1 gin. tnol. KBr per liter and the upper 0.03 gin. 
mol. per liter. 
SOLUBILITY op POTASSIUM BROMIDE IN AQUEOUS SOLUTIONS OF URETHAN AT 25. 

to, 19P8, 19P9.) 



Cte. Mols. per^lOOO as, H^O Solid 

r '~~ ~~ 



o.o 5.797 KBr 

1.1225 5.6l6 " 

7.215 4.886 

14.60 4.421 " + NH-COOCJL 

53.09 o.o NH p COOC p H 5 

SOLUBILITY OF POTASSIUM BROMIDE IN ALCOHOLS AT 25. 

(de Bruyn Z.physik. Chem. io s 783, '92; Rohland Z* iinor^. Chcm. 18, 327, '98.) 

Grams KBr Dissolved by 100 Gms. Alcohol at: 
Alcohol. 



Room Temp. (R.). 25 (dc B.). 

Methyl Alcohol i .92 1.51 Abs. Alcohol 

Ethyl Alcohol 0.28 (Sp. Gr. 0.81) 0.13 " 

Propyl Alcohol 0-055 

100 gms, methyl alcohol dissolve 2.17 gms. KBr at 25. (Turner and Bispctt, 1913.) 
" ethyl " " 0.142 gm. " 

propyi " " -0.035 " 

amyl " " 0.003 " 

SOLUHILITY OP POTASSIUM BROMIDE IN METHYL ALCOHOL. 

'Lloyd, Brown, Olynwyn, Bonnell and Jones, 1920.) 



o 


Qms. KBr per 
100 gros CHjDH 


t 


Qms. KBr per 
100 gms. CH^( 





1.82 


30 


2.23 


10 


1.93 


40 


^.37 


15 

20 


2.00 
2.03 


50 

60 


2-55 
2.74 



SOUJHTUTY OF POTASSIUM BROMIDB IN METHYL ALCOHOL, 
ETHYL ALCOHOL AND j> BUTYL ALCOHOL. 

(Gernuth, 1931.) 

Gms. KBr per IQQ gms. sat. solution in: 

t ' -" 



20 2.5/|2 O.t|53 0.0112 

30 2.496 O.S01 0.0130 

HO 2.440 0.563 0.0137 

50 2,316 0.568 0.0148 



695 KALIUM 

SOLUBILITY OP POTASSIUM BROMIDE IN WATER AND IN SEVERAL ALCOHOLS AT 25- 

(Larson and Hunt, 1939.) 



Solvent 

Water 

Methanol 

Ethanol 
i-Propanol 
i-Butanol 
2- Prop an ol 
2-Methyl-i-propanol 
i- Peritanol 
2-Butanol 



Foraula 



H ? 
OLOH 
Cpfl.OH 
CH CfTCILOII 

ar (cL) ? cn on 

CHlCllOfiCH 



CK 3 C![ ? CHOIICH 3 



d of 
sat. sol. 



0.8025 
0.7861 
0.8010 
0.8058 
0.78lO 
0.7980 
0.8096 
0.8022 



Gma. KBr per 
100 ns. solvent 

67.75 
2. 11 
0.135 
0.031/f 
0.0132 
0.0110 

o. 0076 
0.0048 

0. 0044 



SOLUBILITY OP PoTAvSSiun BROMIDE IN ACETONE. 

(Lannung, 193?.) 



d of 
sat. sol. 



Om. Mol. KBr 
per liter sat. sol. 



0s. KBr per 
liter sat. sol. 



18 
37 



0.792 
0.770 



0.000239 
<J. 0002 12 



0.0359 
0.0328 



SOLUBILITY OF POTASSIUM BROMIDE IN ACETONE AND IN ACETONE 
SOLUTIONS OF SEVERAL SALTS AT 25. 

(Robinson, 19?8.) 



Br 



Added an. Equlv. . On. Equlv. KBr 

Salt, salt. per liter per liter sat. sol. 



Added Om. Equlv. Om. Equlv. KBr 

Salt salt per liter per liter sat. soL 



None (= Pure Acetone) 0.00036 9 $=.044^) KI 
BaRr ? 0.000240 0.000430 " 

" 0.000730 0.000482 " 

11 0.001206 0.000531 Nal 

BaI 2 0.000137 0.000424 " 

" 0.000408 0.000510 " 

" 0.001206 0.000623 " 

SOLUBILITY OP POTASSIUM BROMIDE IN 95% ETHYL ALCOHOL 

CONTAINING INCREASING AMOUNTS OP HYDROBROMIC ACID AT 25. 

(Yaeoda, 1330.) 



0.000343 
0.000877 
0.001763 
0.000382 


0,000414 
0,000489 
0.000579 
0.000418 


0.000939 

o .001849 

0.003542 


0.000494 
0.000571 
0.00065'' 



Normality of HBr 
in 35* C ? h s OH 

0.0 
0.05 
0.10 
0.204 



a of Qras. KBr per 

sat. sol. 100 gros. solvent 



0.7997 
0.805 
0.810 
0.820 



0.289 
0. 191 

o. 165 
0.162 



Normality of HBr 



0.400 
0.537 
0.800 
0.954 



d of Oms. KBr per 

sat. sol. 100 gs. solvent 



0.839 
0.853 
0.878 
0.893 



o . 176 
o. 186 
0.190 
0.242 



The composition of the homogeneous mixture (plait point) of the system 
composed of: 

Potassium Bromide + tertiary Butyl Alcohol + Water at 25 vras found 
by Ginnings, Herring and Webb, 1933, to be: 

11.5 percent KBr + 35.1 percent ter. (CH 3 ) 3 COH + 53-4 percent \l ? 
The originaJ results lor the remaining points of the binodal curve are 
not given but only the values of a series of arbitrary constants calcu- 
lated from them by means of empirical equations. 



K KALIUM 696 

SOLUBILITY OF POTASSIUM BROMIDE IN SRVRRAL SOLVENTS. 

Ons. K3r per 
Solvent Formula t 10Q ^ so i v ent Authority 

Formic Acid < 9 $%) HCOOH 18.5 23.2 (Aschan, 1913.) 

Furfural C H OCHO 25 0.12 (Walden, 1906.) 

Iso Amyl Alcohol (CM ) ? CH(CH ? ),PH2$ 0.00175 (Yagoda, 1930.) 

Hydroxylamine NH^QH ' 17-18 44 . 7 (de Ilruyn, 1892.) 

Hydrazine NH P .NH 2 Ca20 60.0 (Welsh and .Erode rson, 

1915-) 
Ammonia lliquid) NH 3 -33. 9 (d = 0.9098 ) *o. 32 (Johnson and Kromboltz, 

1933- ) 
" " " o 26.87 (Linhard and Stephen, 

1933. 1934.1 

" " " 25 13-50 (Hunt, 1932.) 

Sulfur Dioxide (liquid) S0 g o 2.81 (Jander and Ruppolt, 

1937.) 

PusiON-poifcx DATA FOR MIXTURES OF KRr AND OTHER SALTS. 

KBr * KF (FCurnakow and Wrzesnewsicy, 1912; Ruff and Plato, 1903.) 
KBr + KC1 (Wrzesnewsky, 1912; Amadori and Pampanini, 1911; Ruff and 

Plato, 1903; Tammann and KringS, 1923.) 
KBr + KI (VTrzesnewsky, 1912; Amadori and Pampanini, 1911; Ruff and 

Plato, 1903.) 

Br KRr + NaCl (Ruff and Plato, 1903.) 
KBr 4- KOH (Scarpa, 1915.) 
KBr + KKQ, 

KBr * RbCl (Tammann and KrinpS, 3923.) 
KBr + SrBr g (Kellner, 1917.) 
KBr + TlBr (Rostowski, 1929. ) 
KBr + T1N0 3 

POTASSIUM lodo D1RROUIDR KIBr^ 

One gm. H^O dissolves 10-12 gms. KIBr ? , at 18. 

One liter sat. solution of Potassium lodo di bromide in carbon tetra- 
chloride, contain 0.01173 gnu mol. (?) KIBr g at 25. (Cremer and Duncan, 
1931-) 
POTASSIUM StannoBROMIDES Mono KSnBr 3 .H 2 0, Tetra K^SnBr 4 .H 2 0. 

SOLUBILITY OF MONO POTASSIUM STANNO BROMIDE IN WATER. 

( Rimhaoh and Fleck, 1916. ) 
Gms. per 100 gins. sat. sol. 

t". Itr -f- Sn + K as SnBr a K Solid Phase. 

0.2* ........... ii. 21 3-88 5.94 KSnBr 3 .H 2 0-f-SnBr 8 ,H 2 

17.1* ........... 16.17 6.o5 3.94 

36.3* ........... 2'4.56 10.84 4.90 

46.3.. ......... 3o.83 15.22 5.09 Si.i/f KSnBr 3 .H,0 

74.6 ............ 4o.88 20.^4 6.70 67,82 

SOLUBILITY OF TETRA POTASSIUM STANNO BROMIDE* IN WATER. 

( Ilimback and Fleck, 1916. ) 
Gms. per 100 gms. sat. sol. 

Solid Phase. 

K i SnBr i .H 2 0-+-SnBr 3 .H 2 



t. 
0.3* 


Br -4- 
19.26 


Sn -f- 
1 .00 


K 

8 


16.4* 


28.62 


2 33 


19 48 


43.3* 


33.38 


4 28 


i3.5i> 


62.1* 


3q.43 


8 44 


i3.75 


77-1" 


43.76 


12.73 


i3.o3 



* At these temoeratures the atomic ratios of the constituents in solmifm do not oorrfisnond in 



a . 


"Water. 


Solution. 


* 


o 


3- 1 


3.0 


40 


10 


4.8 


4 .6 


50 


20 


6.9 


6-5 


00 


25 


8.0 


7-4 


80 


30 


95 


8.7 


100 



697 KALiUM K 

POTASSIUM BROMATE KBrO,. 

SOLUBILITY IN WATER. 

(Kremers Pogg:Ann. 97, 5> 's6; Rammelsberg Ibid. 55, 79, '42; Pohl Sitzber. Akad. Wiss 
Wien. 6, 595, '51.) 

Gms. KBrOa per 100 Gms. ft Gms. KBrOa per 100 Gma. 

Water. Solution." 

13.2 ii. 7 

17.5 14-9 

22.7 18.5 

34-o 25.4 

S- 33-3 

Sp. Gr. of solution saturated at 19.5 1.05. 
The following more recent determinations are by Ricci, 1934. 

d of sat. ana. KBr0 3 per Q d of sat. cms. KBr0 3 pr 

c solution too 0s. flat. sol. c solution 100 0ns. sat. sol. 

5 1.024 3.642 30 1.062 8.785 

10 1.035 4.510 35 1.074 10.13 

IS 1.042 5.397 40 1.083 11.58 

20 1.048 6.460 45 13.08 T> o 

25 1.054 7.533 50 14.69 



The following determinations of the solubility of Potassium Bromate 
in Water at temperatures above 100, made by the synthetic method, are 
given by Renrath, Gjedebo, Schiffers and Wunderlich, 1937. 

fas. K3r0 3 per Q fas. KBrO ? per Q fas. KBr0 3 per 

1 100 0ns. sat. sol. l 100 0as. sat. sol. c 100 0as. sat. sol. 

134 43*6 186 59.9 265 77.2 

149 48.4 204 64.2 279 8l.l 

160 51.1 226 70.6 297 83.1 

170 54.1 249 72.6 312 86.4 

EQUILIBRIUM IN THE SYSTEM POTASSIUM BROMATE, POTASSIUM 
CHLORATE AMD WATER AT 25. 

(S wen son and Pled, 1939.) 



. . 

sat. gas, sat, sol. Soild sat. ons. sat. sol. Soll<1 

* 



of fas. pur 100 d. of Gtas. per 100 

t. gas, sat, sol. Soild sat. 

801. ' KBr0 3 * KC10 ? X Ph&se sol. 

1.054 7.533 o.o KBr0 3 1.072 4.02 6.75 882(96.0) 

-- 6.46 2.26 $81(0.46) 1.064 2.79 7.o8 " (97.2) 

1.067 5.75 4.08 " (l.io) 2.07 7.26 " (98.3) 

5.63 4.29 " (2.0) 1.053 1.02 7.6o " (99.1) 

1.078 4.945 6.531 " * 882 1.048 O.o 7.895-KC10 3 

551 " Solid Solution of KC10 in KBrO with a limit of 3* KCICL. 

552 = Solid Solution of KBrO'., in KC10, with a limit of 5'* KRrCL.- 
The figures in parentheses show the percentage of KC10 3 in the solid 

solutions. 



K KAL1UM 



698 



SOLUBILITY OP POTASSIUM BROMATE AT 25 IN AQUEOUS SOLUTIONS OP: 

(Rlccl, 1934.) 



Potassium Chloride 



Potassium Iodide 



d of 


Gtas. per 100 


gjns. sac. 


sol. Solid 


d. of 


Qns. per 100 


9ns. sat. sol 


Solid 


at. sol. 


' KBr0 3 


KC1 


* Phase 


sac. sol. 


KBr0 3 


KC1 


v Phase 


1.054 


7.533 


0.0 


KBrO, 


1.054 


7-533 


0.0 


KBr0 3 


1.058 


4.63 


4.33 


II 


1. 103 


4-54 


8.77 


" 


1.082 


3-24 


9.03 


" 


1.182 


2.96 


18.85 


" 


1.112 


2.44 


14.45 


n 


1.278 


2. 17 


28.60 


n 


1.147 


1-97 


19.71 


n 


1.402 


1.63 


38.99 


11 


1.183 


1.65 


24.87 


n 


1.565 


1.21 


50.06 


11 


1.192 


1.6l 


25.89 


" + KBr 


1.707 


0.99 


58.14 


" 


1.187 


1.48 


25.93 


KBr 


1.729 


0.96 


59.20 


" + KI 


1.179 


0.0 


26.36 


" 


1.718 


0.0 


59.76 


KI 



BrO 



Potassium Nitrate 



5.05 
11.10 
16.98 
23.17 
27.01 
27.27 
27.71 



Potassium Sulfate 



d of 


ana. per \ 


sat. sol. 


' KBr0 3 


1.074 


5.6l 


1. 110 


4.64 


1.148 


4.23 


1. 193 


4.00 


1.225 


3-90 


1.211 


2.64 


1.193 


0.0 



Solid 


d of Oms. per 100 


gws. sat. sol. Solid 


1 Phase 


sat. sol. ' 


KBr0 3 


V4 


v Phase 


KBrO, 


1.066 


6.08 


2.67 


KBr0 3 


II 


1.083 


5.02 


5-44 


II 


II 


1.100 


4.27 


8.20 


II 


II 


1.108 


4.00 


9-35 


" + K SO 


" + KN0 3 


1.103 


3.40 


9.45 


K SO 


KNO S 


1.094 


1.69 


10. 12 


" 


n 


1.083 


0.0 


10.76 


" 



SOLUBILITY OF POTASSIUM BROMATE IN AQUEOUS SOLUTIONS OF VARIOUS 
COMPOUNDS AT 25. 

(Rothmund, 1910.) 



Solvent, 0.5 Normal T 
Aq. Sol. of: * 


CBrOg per 
Liter. 


Cms. 
KBr0 3 per 
Liter. 


Solvent, 0.5 Normal 
Aq. Sol. of: 


Mols. 
KBr0 3 per 
Liter. 


Cms. 
KBrOjper 
Liter. 


Water alone 


0.478 


79.84 


Dimethylpyrone 


0.478 


79.84 


Methyl Alcohol 


0.444 


74.16 


Ammonia 


0.445 


74.33 


Ethyl Alcohol 


0.421 


70.33 


Dimethylamine 


0.384 


64.13 


Propyl Alcohol 


0.409 


68.31 


Pyridine 


0.415 


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 


0-395 


65.98 


Pormamide 


0-473 


79.02 


Formaldehyde 


0.397 


66.31 


Acetamide 


0.445 


74.33 


Glycol 


0.448 


74.84 


Glycocol 


0.501 


83.68 


Glycerol 


0.451 


75.34 


Acetic Acid 


0.456 


76.17 


Mannitol 


0.451 


75-34 


Phenol 


0.426 


7LI5 


Grape Sugar 


0.431 


71.99 


Methylal 


0.405 


67.66 


Urea 


0.477 


79.68 


Methyl Acetate 


0.420 


70.15 



699 KALiUM K 

SOLUBILITY OP POTASSIUM BROMATE IN AQUEOUS SOLUTIONS OF 
SODIUM NITRATE AND OF SODIUM CHLORIDE. 

(Geffcken Z. physik. Chem. 49, 296, '04.) 

In Sodium Nitrate. In Sodium Chloride. 

Grams per Liter. Mols . KBrOa Grams per Liter. Mo j s . K BrO 3 

NaNO 3 . KBrO 3 . Per Liter. NaCl. KBrO 3 . Pe r Liter. 

0-0 78.79 0.4715 0-0 78.79 0.4715 R A 

42-54 96.01 0.5745 29 25 82.24 0.5220 

85-09 108.6 0.6497 5^-50 93-87 0.5616 

170.18 128.3 0.7680 117.0 100.9 0.6042 

2 55- 2 7 ^o-Q 0.9026 I 75-5 104.3 0.6244 

340.36 172.3 1.031 234.0 106.9 0.6400 

TOO gms. liquid Ammonia dissolve 0.002 gm. KBrO at 25. (Hunt and 
Boncyk, 1933.) 
POTASSIUM METHIONATE K 2 ^ CH 2 ' (S0 3 ^ 

100 gms. sat. solution of Potassium Methionate in Water contain 4.46 
gms. K ? [CH g (SI 3 ) ? ] at 25 o^ (Backer, 1929; Baker and Terpstra, 1929. ) 

POTASSIUM Chlor MBTHIONATE K.[CHC1 (SO, ) J 

c o fT 

100 gms. sat. solution of Potassium Chlor Methionate in water contain 
3^.2 gms. KglCHCl(S0 3 ) g J at 25. (Raker, 1930.) 

POTASSIUM FORMATE HCOOK. 

Determinations of the freezing-points of aqueous solutions of potassium formate 
made in a Beckmann apparatus, gave the following results. 

t 2. 02. 0.72. 10.42. 1S.82. 17.:9. ^H 

Gms, HGOOK per 100 gms. sat. sol.. . 6.71 12.96 18.4-2 25. o3 26.04 
The solid phase was ice in all cases. ( Sid g wick and Gentle, 1022. 

SOLUBILITY OF POTASSIUM FORMATE AND OF T&E ACID SALT IN WATER. 

(Groschuff, 1903.) 
Solid Phase : HCOOK. Solid Phase : HCOOK.HCOOH. 



Gms. 
HCOOK 

t. per zoo 
Gms. 


Mols. 
HCOOK 
per 100 
Mols. 


^Gms. HCOOK 
HCOOH 
t. per loo 
Gms. 


Gms. 

HCOOK: 

per 100 t. 
Gms. 


Gms. 
HCOOK 

per 100 
Gms. 


Mols. 
HCOOH 
per i 
Mol. 


Solution. 


H 2 0. 


Solution. 


Solution. 


Solution. 


HCOOK. 


20 


72 


.8 


57 


4 


O 


60.4 


39 


.0 





3^3 


3 .2I 


+ 18 


76 


.8 




.0* 


2 5 


69.8 


45 


.1 


19-5 


38.2 


2 .96 


5 


80 


7 


89 


.8 


50 


79-2 


5 1 


.2 


39-3 


40-8 


2 .65 


90 


86 


.8 


141 


.0 


80 


90.7 


58 


.6 


60 


44-o 


2-33 


1 20 


92 


.0 


247 


.0 










70 


45-9 


2.16 


140 


96 


.0 


511 












90 


52-1 


1.68 


157 


100 


.0 


CO 



















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. 

Freezing-point data for the system HCOOK + HCOOH are given by Kendall 
and Adler, 1921. 



K KALIUM 700 

POTASSIUM ACETATE CH 3 COOK. 

Determinations of. the freezing-points of aqueous solutions of potassium acetate 
made in a Beckmann apparatus gave the following results : 

t" 2. is. :j.:ifi. O.Hi. 12.32. 17.02. 

Gms. GH 3 COOK per too gms. sat. sol... 5.oo 7.42 17.04 2O.5& i5.5 
The solid phase was ice in all cases. (Sidgwick and Gentle, 1922.) 

ioo gms. aq. 86.5/ Glyccrol (d = 1.2826) dissolve 77.4 gms. CH 3 COOK at 20. 
qB.5/o (rf = i.a645) 6o.5 

( Holm, 1921, 1022. ) 

Data for the freezing-points of mixtures of potassium acetate (m. pt. 296) and 
sodium acetate (m. pt. 820) are- given by Baskof, 1916, 1917. The salts form solid 
solutions in all proportions and no eutectic point was obtained. The lowest 
i. pt., 233, was found for a mixture containing 46 mol. per cent CH 3 CO Na, 

Data for the freezing-points of mixtures of potassium acetate and 
lead acetate are given by Lehman and leifer, 1938. 

POTASSIUM ACETATE CH 3 COOK.iJH 2 O. 

SOLUBILITY IN WATER. (Abe, 1911.) 

Cms. CH S COOK Gms. CHjCOOK 

t. per ioo Grns. Solid Phase. t. per ioo Gms. Solid Phase. 

H0. H a O. 

O.I 216.7 2CHjCOOK.3H 2 O 41 3 2 7-7 2 CHjCOOK.aHsO 

5 223 .9 41 .3 tr. pt. ... + 2 CH 3 cooK.H,o , 

10 233.9 " 42 329 aCHjCOOK-H^O 

CH 15 2 43-i " 45 332.2 

20 255.6 " 50 337.3 

25 269.4 " 60 350 

30 283.8 " 70 364.8 

35 301.8 80 380.1 

38 314.2 90 396.3 

40 323.3 " 96 406.5 

SOLUBILITY OF POTASSIUM ACETATE IN AQ. ALCOHOL SOLUTIONS AT 25. (SeideU,'io.) 

\Vt. % C 2 H,OH </ 28 of Gms. CH,COOK per Wt. % CaH 6 OH rfj, of Gms. CH,COOK per 
in Solvent. Sat. Sol. ioo Gms. Solvent. in Solvent. Sat. Sol. ioo Gms. Solvent. 

o 1.417 219.6 70 1.156 118.3 

20 1.363 219.6 80 1.685 87.6 

40 1.302 192.4 90 0.990 52.9 

50 1.260 171.8 95 0.922 34.2 

60 1.210 147-5 IO 0.850 16.3 

SOLUBILITY op POTASSIUM ACETATE IN ACETIC ACID, DETERMINED 

BY THE FREEZING-POINT METHOD. 

(Davidson and McAllister, 1930.). 

On. Mols. CH ? COOK per Solia Q fta. Moia. CH^COOK per Solid 

1 100 90. mols. mixture Phase c 100 am. nola. rail cure Phaae 

16.50 o.o CHgCOOH 110.0 30.67 1.1 

15.82 1.22 " Il8.0 32.47 " 

10.95 6.70 " 124.5 34-41 " 

7.45 9.10 " 126.0 35.27 " 

5-95 10.03 " 137.0 39.5 " 

14.76 10.97 1.2 145.0 44-38 " 

28.03 12.71 " 147.5 48.30 " 

49-90 15.75 " 148.0 50.22 " 

64.1 18.71 " 147.5 52.32 " 

73.5 20.48 " 170 58.45 CH 3 CXX)K 

83.6 23.85 * 206 64.16 

99.0 28.44 1.1 245 76.50 " 

292 ioo. oo " 

1.2 = CH 3 COOK. 2 CH 3 COOH; 1.1 = CH 3 COOK.CH 3 COOH 



70T KALIUM 

The following results, differing from the above were obtained by 
Bakunin and Vitale, 1935. 

On. Mols. (UNCOCK Solid Q On.- Mols. CHgCOOK Solid 

1 per 100 gm. raols. mixture Phase l per 100 gm. mols. mixture Phase 

16 o.o CHjOOOH 134 42.88 2.1 

9 5.23 " 138.6 50.06 " 

3 10.33 " 147 58.05 CH 3 COOK 

o Butec. "+ 1.2 175 60.20 "" 

14 16.22 1.2 234 71.83 " 

64 23.43 2.1 258 81.73 " 

101 29.43 " 292 98.24 " 

112 37.27 " 297 100.00 " 

100 gms. methyl alcohol (CII 3 OH) dissolve 24.24 gms. C1I 3 COOK at 15 

and 53.54 gms. at 73.4 (= b. pt. of the sat. sol.). The salt gives 

extremely hygroscopic crystals of the alcoholate, CH 3 COOK.CH 3 OH. 

(Henstock, 1934.) 

100 gms. liquid Ammonia dissolve 1.026 gm. CH 3 COOK at -33. 9 . 

(Johnson and Krumboltz, 1933.) 
100 gms. liquid Sulfur Dioxide dissolve 0.006 gm. CH 3 OOOK at o. 

(Jander and Ruppolt, 1937.) 

POTASSIUM PROPTONATE C^HgCOOK.H^O 

100 gms. methyl alcohol (CH 3 OH) dissolve 39.0 gms. anhydrous potassium 
propionate at 15 and 55.33 gms. at 7i.3*(* b. pt. of sat. sol.). 
(Henstock, 1934.) 
POTASSIUM BUTYRATE C,H 7 COOK. 

loo gms. water dissolve 296.8 gms. CjH 7 COOK, or 100 gms. sat. solution con- 
tain 74.8 gms. at 31.25. 

100 gms. of an aq. solution saturated with sugar and CaHyCOOK contain 
49.19 gms. sugar -f- 34.78 gms. C 3 H 7 COOK -f 16.03 gms. H 2 O at 31.25. 

(Kohler, 1897.) 

100 gms. methyl alcohol (CH 3 OfI) dissolve 51.04 gms. n potassium 
butyrate, CH ? CH e CH 2 COOK, at 15 and 120.84 g ms - a t 70.9* (= b. pt. sat. 
sol.). (Henstock, 1934.) 
POTASSIUM Iso BUTYRATE (CH ? J^CHCOOK 

EQUILIBRIUM IN THE SYSTEM POTASSIUM Iso BUTYRATB, 
Iso BUTYRIC ACID AND WATER AT 25. 

(Bury and Menas, 1939.) 

Suitable mixtures were shaken in Hard glass vessels until analysis 
showed that equilibrium was established. Iso" butyric acid was deter- 
mined by tit rat ion and potassium iso butyrate by conversion into 
potassium chloride. The two liquid layers which were formed in all 
cases had the following compositions. 

Upper Layer Lower Layer Upper Layer Jxwer Layer 

Gas. per 100 tps. Qma. per 100 SUB. Ons. per 100 pas. Ctas. per 100 ^s. 

sat.^801. aat.^aol. sat. A ol. 8ac. A aol. 

jO 



57.26 





24.0 





51-20 


0.2" 


30. 17 


0.32 


57.08 


0.02 


24.23 


0.09 


49.8l 


0.23 


30.99 


0.33 


56.90 


0.05 


25.09 


O.l8 


49.00 


0.24 


31.21 


0.34 


55.54 


0.08 


26.43 


0.23 


47-91 


0.26 


31.80 


0.34 


54.76 


0. 10 


27-H 


0.25 


46.89 


0.28 


32.56 


0.34 


53.81 


0.13 


27-72 


0.27 


45-72 


o. 29 


34.02 


0.35 


53.17 


o. 16 


28.00 


0.28 


44. 5H 


0.30 


35-21 


0.36 


52.50 


0.18 


29.03 


0.29 


43.48 


0.32 


37.62 


0.36 



51.72 0.19 29.69 0.30 42.00 0.34 39.57 0.37 

51.11 0.20 30.O8 0.32 



KALIU.M 702 

POTASSIUM TAETEATE (Mono) KHC 4 H 4 6 , Cream of Tartar. 
SOLUBILITY OF MONO POTASSIUM TARTRATE IN WATER. 

(Afluard, 1865; Roelofsen, 1894; Blarez, 1891; at 20, Magnanini, 1901; at 25, Noyes and Clement, 1894.) 

Cms. KHC 4 H 4 6 per 100 
Gms. Solution. 



t. 



Gms. KHC 4 H 4 6 per 10 
Gms. Solution. 



t. 



o 0.30 (R.) 0.32 (A.) 


o.35 (B.) 


40 


0.96 1.3 


1.29 


10 0.37 


0.40 


0.42 


50 


1.25 1.8 


i. 80 


20 o . 49 


o.S3(M.) 


0.60 


60 


2.4 


. . . 


25 0.58 


o.6s4(N. andC.) 


o-74 


80 


4-4 




30 0.69 


0.9 (A.) 


0.89 


100 


... 6.5 





POTASSIUM TARTRATE (Mono) (CH OH) 2 GOOH. COOK (Cream of 

Tartar). 

SOLUBILITY OF MONO POTASSIUM TARTRATE IN WATER. 
(Paul, [at 18, 1917] 192C. ) 

NOTE. A weighed amount of dried tartrate was shaken with a weighed amount 
of water a given time in a thermostat. The undissolved salt was filtered on a 
Gooch crucible, dried over phosphorus pentoxide and weighed. Furthermore the 
content of the solution was determined by titration with standard barium hydroxide 
solution. 





^ Of 


Gms. KHC,H. V C per 




4 of 


t. 


sal. sol. 


100 cc. sal. sol. 


t". 


sat. sol. 


Q 


i ooiA5 


o 2653 


18 


I . OO I 2O 


5 


i 002*^4 


o./ion^ 




I.OOIOO 


[o 


I OO I 80 


0.3663 


25 


r . 00079 


I/!.... 


, . I. 00 IT2 


o.43oi (4.8V l) 


3o 


i . 00026 



per 
JOO gins. sat. sol. 

0.4896 

0.5337 (o.54l5) Cl) 

o.64t2 

0.7623 

(i) This result is by Pierrat, 1921 ; (2) This result is by Moser and Ritschel, 1925. 



Later very careful determinations by Carpenter and Mack, 1934, gave 
the following results: 





a or 


Oms. KHC^H^Og per 




d. of 


3B8. KHC H.O. per 


t 


sat. sol. 


100 gs. sat. sol. 


t 


sat. sol. 


100 BNS. sat. sol. 





1.0012 


0.2305 


15 


1.0016 


0.4338 


5 


1.0016 


0.2870 


20 


1.0012 


0.5323 


10 


1.0020 


0.3579 


25 


1.0003 


0.6412 



SOLUBILITY OF MONO POTASSIUM TARTRAT* IN AQUEOUS 
SOLUTIONS OP KBUTRAL DiPoiASsiUM TARTRATB AT 20. 

(Rlchert, 1930.) 



Oft. Hols, per : 



of sat, solution 



Ote. Hols, per llte^of sat, solution 





"We x 


W4e 


KHC 4 H 4 O fl 


0.000 


0.0284^= 5-342 gms. 


) 0.00443 


0.00667 


0.000443 


0.0218 1 


0.00714 


0.00540 


0.000886 


0.0176 


0.0143 


0.00360 


0.00177 


0.0124 


0.0214 


0.00280 


0.00266 


0.0096 


0.0286 


0.00264 


0.00354 


0.00805 


0.0357 


0.00260 



703 



KALIUH K 



POTASSIUM Acid TARTRATE KHC.H.O. 

446 

SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS SOLUTIONS 
op NEUTRAL Di POTASSIUM TARTRATE AT SEVERAL TEMPERATURES. 

(Carpenter and Mack, 1934.) 



Qma. Kj,C 4 H 4 Q per 
100 gms. sac. sol. 

0.00 

0.025 

0.050 

0.100 

0.200 

0.300 

0.400 

0.500 
0.600 
0.700 
0.800 

Oma. KgC 4 H 4 O e per 
100 ms. sac. sol. 

0.00 

0.025 

0.050 

0. 100 

0.200 

0.300 

0.^00 

0.500 

0.600 

0.70.0 

0.800 



GBS. KHC 4 H 4 O e par IQO^gms. sat, solution 



t 







5 


10 


\ 


0. 


2305 


(l 


.0012) 





.2870 


(1 


.0016) 


0. 


3579 


(l 


.0020) 


0. 


2010 


(1 


.0010) 





.2562 


(l 


.0016) 


0. 


3272 


(l 


.0020) 


0. 


1772 


(1 


.O009 ) 





.2322 


(1 


.0017) 


o. 


3000 


(1 


.0021 ) 


0. 


1394 


(1 


.0011) 





.1936 


(1 


.0021 ) 


0. 


2557 


fl 


. 0024 ) 


0. 


0978 


(l 


.0014) 





1437 


(1 


.0025) 


o. 


1924 


(1 


.0027) 


0. 


0758 


(l 


.0018) 





.1098 


(1 


.0029 ) 


0. 


1540 


(l 


,0030) 


0. 


0617 


(1 


.0024) 





.0902 


(l 


0035) 


0. 


1317 


(l 


. 0036 ) 


0. 


0523 


(1 


.0031 ) 





.0784 


(l 


. 004 1 ) 


0. 


1143 


(1 


.0042) 


0. 


0480 


(1 


.0038) 





.0703 


(1 


.0047) 


0, 


1039 


(1 


.0048) 


0. 


0433 


(l 


.0046) 





.0638 


(1 


.0053) 


0. 


0935 


(l 


.0054) 


0. 


0379 


(1 


.0052) 





.0562 


(1 


.0059> 


0. 


0824 


(1 


.0060) 


Oms. KHC 4 H 4 6 per lOO^gjns. sat. 


solution at: 


' 




15 


20 


25 1 


0. 


4338 


(l 


.0014) 





.5323 


I 1 


.0012) 


0. 


6412 


(l 


.0003) 


0. 


4050 


. (l 


.0017) 





.5010 


(l 


.0012) 


0. 


6l20 


(l 


.0003) 


0. 


3793 


(1 


.0017) 





.4737 


(l 


.0013) 


0. 


5894 


(l 


.OO04) 


0. 


3307 


(1 


.0018) 





.4228 


(1 


.O014) 


0. 


5424 


(1 


. 0006 ) 


0. 


2651 


(l 


.0021 1 





.3492 


(l 


.0016) 


0. 


4560 


(1 


.0008) 


0. 


2186 


(1 


.0025 ) 





2939 


(1 


.0020) 


0. 


3898 


(l 


.0011) 


0. 


1890 


(1 


.0028) 





.2532 


(1 


.0021 ) 


0. 


3428 


(l 


,0015) 


0. 


1652 


(l 


.0031 ) 





.2208 


(\ 


.0023) 


0. 


3060 


(1 


.0020) 


0. 


1492 


(1 


.0037) 





.1977 


(1 


.0025) 


0. 


2773 


(I 


.0022) 


o. 


1357 


(1 


.0041) 












0. 


2522 


ll 


.0024) 


0. 


1220 


(1 


.0149 












0. 


2292 


(l 


.0028) 



C 4 H 



The figures in parentheses are the densities of the saturated solutions. 

SOLUBILITY OP MONO POTASSIUM TARTRATE IN AQUEOUS 
SOLUTIONS OF TARTARIC ACID AT 20. 

(Richert, 1930.) 



Om. Mola. per liter sat. solution 



' H ? C 4 H 4e 


KHC 4 H 4 O e i 


0.0030 


0.0268 


0.0055 


0.0260 


0.0105 


0.0240 


0.0335 


0.0238 


0.0485 


o . 0238 



KALI DM 704 

SOLUBILITY OF MONO POTASSIUM TARTRATK IN AQUEOUS SOLUTIONS 
OF TARTARIC ACID AT SEVERAL TEMPERATURES. 

(Carpenter and Mack* 1934.) 



Ons. KHC 4 H 4 O e per 100 gojfr. sat, solution at: 



100 



as. sat. aol. 

0.0 

0.025 

0.030 

0.100 

0.200 

0.t).00 

0.600 

0.800 






10 


26 


0.2305 (1.0012) 


0.03579 (1.0020) 


0.6412 (1.0003) 


0.2162 (1.0013) 


0-3457 (1.0O20) 


0.622O (1.0003) 


0.-207S (1.0013} 


0.3352 (l.002i) 


0.6063 (l.OOOq.) 


0.1962 (1.0014) 


0.3205 (l.OO2l) 


0.5842 (1.0005) 


0.1842 (l.00l6) 


0.3003 (1.0026) 


0.5558 (1.0008) 


0.1680 ( 1.002(0 


0.2715 (1.0033) 


0.5243 (1.0014) 


0.1600 (1.0035) 


0.2502 (1.0042) 


0.498l (1.0021) 


0.1503 (l.OOq?) 





0.47l6 (1.0027) 



The figures in parentheses are the densities of the saturated solutions. 



SOLUBILITY OF MONO POTASSIUM TARTRATE 

SOLUTIONS OF ACIDS AT 20 

(Ostwald; Huecke, 1884.) 



IN NORMAL 



Purified tartrate was added in excess to normal solutions of the acids, and, after 
shaking, clear I cc. portions of each solution were withdrawn and titrated with 
----- ' o.i n Ba(OH)2 solution; i cc. normal acid requiring 10.63 cc. of 



the Ba(OH) 2 solution. 

Gins. cc. N/io 
A ., Acid Ba(OH)a 


Cms. 
KHC^HiOg 


\ Arid 


Gms. cc. N/TO Oms 
Acid Ba(OH) 3 KHC*!-!^ 


Aad * per i oo cc. 
Solvent. 


per T cc. 
Solution. 


per too cc. 
Solution. 


Acia> pert oo cc. 
Solvent. 


per ice. perrcocc 
Solution. Solution" 


HNO, 


6. 


3 1 


5- 


77* 


10.21 


C 2 H 5 S0 3 H 


II, 


.0 


5- 


.01* 


8.87 


HCi 


3. 


65 


5- 


3 2 


9.42 


HO.(CH 2 ) 2 S0 3 H 


12. 


61 


5- 


33 


9-43 


HBr 


8. 


IO 


5- 


38 


9-75 


C 6 H 5 S0 3 H 


15. 


81 


5. 




9.29 


HI 


12. 


80 


5- 


43 


9.61 


HCOOH 


4. 


60 


0. 


45 


0.80 


H 2 SO< 


4- 


90 


3- 


97 


7-03 


CH 3 COOH 


6 


.00 


o. 


.27 


0.48 


HCH 3 SO 4 






5- 


58 


12.44 


CH 2 C1COOH 


9- 


45 


I. 


01 


1.79 


HCJ^SO, 


12. 


61 


5- 


4i 


9-58 


C 2 H,COOH 


7 


.40 


0. 


24 


0.42 


HC 3 H 7 S0 4 


14. 


OI 


5-2i 


9.22 


C 3 H 7 COOH 


8. 


81 


o. 


2 3 


0.41 



* The figures in this column show the amount of the Ba(OH) 2 solution in excess of that which would 
have been required by the normal acid solution alone in each case, viz., 10.63 cc. They, therefore, corre- 
apond to the amount of KHQHtOe dissolved in i cc. of each saturated solution, and when multiplied 
by i-77give the grams of KHC^Oa per 100 cc. solution. 

SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS SOLUTIONS OF VARIOUS 
SALTS AND ACIDS AT 13 TO 15. (Klapprotb, 1022.) 

The method used for securing saturation consisted (A), in dissolving i.o gram 
of KH C 4 H 4 O 4 in hot water and adding the solution to the quantity of salt or 
acid necessary to yield the concentration in which it was desired to determine the 
solubility of the tartrate. The mixture was diluted to 100 cc., shaken frequently, 
allowed to cool to room temperature and stand at least one day. An alternate 
method (B) differed from the above only in that the i.o gram of tartrate was added 
directly without previously being dissolved by warming. Thus an attempt was 
made to approach equilibrium from above and from below without application 
of continuous agitation. The results by the two methods differ so greatly that 
it is certain saturation was not reached. Consequently, the figures have only a 
qualitative interest. They show, in general, that salts with a common ion reduce 
the solubility and acids or salts with no common ion increase it. The solubility 
was found to be least in a formic acid mixture, and it was concluded that this acid 
could be advantageously used to precipitate mono potassium tartrate from its 
aqueous solutions. 



POTASSIUM Acid TARTRATE 



70S 



KALIUM K 



SOLUBILITY OF MONO POTASSIUM TARTRATE (KHC^Oe) IN AQUEOUS 
SOLUTIONS OF ELECTROLYTES AT 25. 

(Noyes and Clement, 1894; Magnanini, 1901.) 



Electro- 


Gm- Equiv. per 
Liter. 


Cms. per 
Liter. 


Electro- 


Gm. Equiv. per 
Liter. 


Gms. per 
Liter. 


lyte. 


Electro KHC 4 * 


Electro- 


KHC 4 


lyte- Electro- 


KHC 4 


Electro- 


KHQ 




lyte. 




HA. 


lyte. 


.HA. 




lyte. 


HA. 


lyte. 


HA. 


KC1 


0.025 


O 


.0254 


1.86 


4.788 


CHsCOOK 


0.05 


o 


.0410 


4.91 


7.718 


it 


0.05 





.0196 


3-73 


3.680 


a 


O.IO 





.0504 


9.82 


9.486 


a 


O.IO 





.0133 


7.46 


2.509 


(t 


O.2O 





.0634 


19.63 


11.930 


tt 


0.20 


0.0087 


14.92 


1.636 


KHS0 4 ( 2 o) 


0.01 


o 


.0375 


1.36 


7.06 


KC10 3 


0.025 


o 


.0256 


3.06 


4.821 


tt 


O.O2 





.0500 


2.72 


9^4* 


tf 


0.05 


0. 


0197 


6.13 


3.716 


tt 


O.IO 


o 


1597 


13.62 


30.06 


tt 


O.IO 


0. 


0138 


12.26 


2 .601 


KHC 2 O 4 * (20) 


O.OI. 


o 


.0369 


1.28 


6.94 


tt 


o. 20 


o. 


0097 


24.52 


1.728 


u 


0.02 





.0424 


2.56 


7.98 


KBr 


0.05 


o. 


0192 


5-95 


3-699 


tt 


o.io 


o. 


.1132 


12.82 


21 .30 


it 


O.IO 


0. 


0134 


11.91 


2.5*7 


HCl 


0.013 


0. 


.0367 


o-45 


6.90 


n 


0.20 


o. 


0087 


23.82 


1.629 


u 


0.025 


o. 


.0428 


0.91 


8.06 


KI 


0.05 


0. 


0196 


8.30 


3-687 


it 


0.050 


0.0580 


1.82 


II.O9 


it 


O.IO 


0. 


0132 


16.61 


2.492 


Nad 


0.05 


0. 


.0376 


2.Q2 


7.08 


tt 


o. 20 


o. 


0086 


33-22 


1.619 


n 


O.IO 


o, 


0397 


5.85 


7-48 


KNOs 


0.05 


0. 


.0195 


5-06 


3.676 


tt 


0.20 


o. 


,0428 


11.70 


8.05 


n 


O.IO 


0. 


0136 


IO.I2 


2.5SI 


NaClOa 


0.05 


0. 


.0382 


5-32 


7.18 


tt 


o. 20 


o. 


0090 


20.24 


1.696 


n 


O.IO 


o, 


,0405 


10.65 


7.63 


K 2 S0 4 


0.05 


0. 


,0208 


4.36 


3.921 


tt 


O.2O 


0, 


.0446 


21.30 


8.40 


u 


O.IO 


0. 


,0147 


8.72 


2.769 














n 


O.2O 


o. 


,0100 


17.44 


1.888 






















* 


= acid potassium oxalate. 



100 gms. Methyl Alcohol. (CHgOH) dissolve 0.6 gm. 
(b.pt.). (Henstock, 1934.) 



at 66 - 



C 4 H 



SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS ALCOHOL AT 25. 

(Seidell, 1910.) 
Wt. ^ 

in Solvent. 


10 
20 
30 
40 



Sat. Sol. 


Gms. KHC 4 HA 
per 100 Gms. 
Sat. Sol. 


Wt. % 
QHiOH 
in Solvent. 


<*25 Of 

Sat. Sol. 


Gms. KHC 4 HA 
per 100 Gms. 
Sat. Sol. 


1.002 


0.649 


50 


0.912 


0.064 


0.985 


0.358 


60 


0.890 


0.043 


0.970 


O. 2IO 


80 


0.842 


0.023 


0-953 


O.I3I 


92.3 


0.807 


0.014 


0-933 


0.087 


100 


0.789 


O.OIO 



SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS SOLUTIONS OF ALCOHOL 

AT 14. (Pierrat, 1921.) 

Saturation was obtained by agitating the mixtures for several hours. The 
sat. solution was evaporated to dryness in a current of air and the residue dissolved 
in enough water to yield the original volume of the solution. The tartrate in this 
was determined by electrolytic conductivity. 



Wt. per cent 
tills Oil in solvent. 

0.0(= H 2 0) 

8. 7 



Gms. 



ms. tin 

per 100 cc. sat. sol. 



4.8 

2.'Jl 
1.5 

0.77 



Wt. per cent 
C,II 5 OII in solvent. 

4^.4 

58.5 
94-7 



Gms KHC4H 4 O fi 
per 100CC. sat. sol. 

0.4'2 
O.2O 
O.05 



KAUUM 706 

SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS SOLUTIONS OF ALCOHOL 
AT l8. (Paul, 1927, 1926.)- 

Gms. 1UIC A 11^00 per lOOcc. sat. solution in.aq. C a If 5 OIT of 

5,0 gms. C S H 5 OH 8.0 gras. C 2 II 5 OH^ "^^^loTo gms. C 4 H 5 OH 

t". per lOOcc. per JOO cc. per lOOcc. 

(dw= o.g865o) (d%& = o.g8i55) (dao = 0.97518 ) 

o 0.1746 (0.98998) 0.1875 (0.98247) 0.1248 (0.97805) 

10.... 0.2605 (0.98974) 0.2078 (0.98203) 0.1905 (0.97746) 

18 0.358 0.294 0.258 

20 0.3924 (0.98876) 0.3371 (0.98170) o.3oo3 (0.97678) 

25 0.4747 (0.98785) o.4o45 (0.98141) 0.3662 (0.97546) 

3o 0.5846 (0.98673) 0.4960 (0.98118) 0.4323 (0.97864) 

The figures in parentheses show the dt of the saturated solutions. 

The author also gives data for the p\\ and the electrolytic conductivity of the 
saturated solutions. 

POTAvSSIUM Acid TARTRATE KHCJLO. 

4 4i 

SOLUBILITY OP MONO POTASSIUM TARTRATB IN AQUEOUS 
SOLUTIONS OF INVERT SUGAR (GLUCOSB + FRUCTOSE) AT 20. 

(Rlchert, 1930.) 

Percent Invtrt Om. Mols. KHC 4 H 4 O e per: 

sugar by weight ^ 


IS 
30 
45 
60 
80 

SOLUBILITY OP MONO POTASSIUM TARTRATB IN AQUTSOUS SOLUTIONS 
OF SBVBRAL SUGARS AT 20. 

(Carpenter and Kucera, 193*0 

Wt. Percent Qas. KHC 4 H 4 6 per 100 gas^ sat, solution in aqueous: 

^gar ' d 01 u co as d Fructose Invert Sugar Sucrose N 

Solution Solution Solution Solution 

o 0.5323 (1.0012) 0.5323 (1.0012) 0.5323 (1.0012) 0.5323 (1.0012) 

s 0.5180 (1.0210) 0.5171 (1.0209) ~" 

10 0.4924 (1.0405) 0.5037 (1.0414) 0.4979 d.0411) 0.4715 (1.0409) 

20 0.4442 (1.0824) 0.4637 (1.0843) 0.4570 (1.0837) 0.4237 (1.0835* 

30 0.4010 (1.1272) 0.4269 (1.1303) 0.41S2 (1.1296) 0.3707 (1.1293) 

40 0.3833 (1.1796) 0.3700 (1.1788) 0.3114 (1.1784) 

The figures in parentheses are densities of the saturated solutions. 
The authors also give similar results for the temperatures o? 5? ioand 15. 

POTASSIUM TARTRATE (K^HUOa^.I^O. 

100 gms. H 2 dissolve 138 gms. KaCJiA at 16.6, Sp. Gr. of sat. sol. = 1.49. 

(Greenish and Smith, 1901.) 



lOOOcc sat. solution 

. 0284 
0.0276 
0.0264 
. 0240 


1000- gms. sat. sol. 

0.0284 
0.0260 
0.0232 
0.0198 


. 0200 
0.0124 


0.0155 
0.0087 



707 KALIUM K 

POTASSIUM Sodium TARTBATE, KNaC 4 H 4 6 .3 H 2 O and.4H 8 r and d. 

SOLUBILITY OF THE POTASSIUM SODIUM SALT OF DEXTRO AND OF 

RACEMIC TARTARIC ACIDS IN WATER. ( Bronsted, 1921, 1926.) 

c , Salt of Mixture 

^jgHj^Hacemlc^Acld-. j ^ ^^Jjfl 1 of pyxtro AcjcL^^ ofrfand / Achfo 

Gms - Gms. Gms. Gms. 

t of KNaC<ir,O c t'of. KNaC 4 H,0 6 for. KNaC 4 H,O a f of. KNaC 4 H 4 6 

tryst. per JOOg-ms. H 2 0. Cryst. per 100 gms.ir s O. Cryst. per lOOgms. ir 2 0. Cryst. per 100 gms. If , 0. 

-6.98... 4-2.7 -4.7 28.7 o.o... 3-2.o -6.42... 89.3 

-5.95... 36.5 -4.34 26.0 9.7... 46. i +9.7 64.4 

+9-7 58.o -3.38 19.0 iS.o... 62.9 29.5 i4o.5 

29.5 92.3 -1.87)... 10.2 29.5... 100.7 

EQUILIBRIUM IN THE SYSTEM POTASSIUM SODIUM TARTRATE 
SODIUM HYDROXIDE AND WATER AT 25. 

f Campbell and Campbell, 1932.) 
fas, per 100 ans. sat. sol. Qns. per 100 gna. aat. sol. 

/ .~. - . .. - ' "" -- -.. V / -^ 

22.6 12.2 

l6.1 1385 

21.6 15.3 

35-2 24.8 

25-7 23.9 

The three sections of the solubility curve are considered to cor- ^4^ 
respond respectively to hydrated Rochelle Salts, anhydrous Rochelle 
Salts and a solid complex which resembles a stiff gel. 



KNaC 4 H 4 6 


NaOH " 


39.0 


0.0 


330 


3-7 


31.0 


5.8 


29.0 
29.5 


7-3 
7.6 


20.2 


13-5 



POTASSIUM Sodium TARTRATE. KNa.C^Aj^HaO. (Rochelle or Seig- 

nette Salt.) 

100 gms. sat. aq. solution contain 36.66 gms. KNaC^^Oc at 9.7 and 47.97 gms. 
at 29.5. (van't Hoff and Goldschmidt, 1895.) 

ioo gms. H 2 dissolve 53.53 gms. KNaC^Oe at 15, Sp. Gr. of sol. 1.2713. 

(Greenish & Smith, 1901.) 

SOLUBILITY OF MIXTURES OF POTASSIUM TARTRATE AND OF SODIUM 
TARTRATE IN WATER AT SEVERAL TEMPERATURES. 

(van Leeuwen, 1897.) 

t n G ms - P 61 " 1 P Gms. Sat. Sol. Gms. per ioo Gms. Sat. Sol. 

' 'K 2 C 4 H 4 6 . ^Na^HA-' l ase ' ' ' K 2 C 4 H 4 O 6 . Na^fL/V ' 

1 8 IQ.2 16.5 KNaC 4 H 4 064H a O 26.6 56 4.2 

38 26.6 22.8 48.3 51.6 13.2 

20.9 II. 8 28 " +Na,T 59.7 44-5 25.3 

38 25.8 24.7 " " 80 39.7 34.7 

50 36.7 23.9 

K-2T = I<2C4H40o.2H2O. NaaT Na2C4H4Oe.2H2O. 
SOLUBILITY OF SEVERAL POTASSIUM SALTS OF TARTARIC ACIDS IN WATER AT 20. 

(Schlossberg, 1900.) 



Potassium Sodium Salt of Racemic Acid KNa(QH 4 6 ) .3H 2 62 .84 

Potassium Sodium Salt of d Tartaric Acid KNafoHA^EW 63 . 50 

Potassium Neutral Inactive Pyrotartrate K 2 C5H 6 06.H 2 O 5^-33 

Potassium Neutral Dextropyrotartrate K^HeOe 57.62 



K KALiUM 708 

SOLUBILITY OF POTASSIUM SODIUM TARTRATE IN AQ. ALCOHOL SOLUTIONS AT 25. 

(Seidell, 1910.) 



Wt. % 
CjHjOH 
in Solvent. 


j ^r Gms. 

S*!sol. KNaC,HA. 4 H 2 
oat. owi. per I00 QJ^ Solvent 


wt. % 

C 2 H 6 OH 
in Solvent. 


j rtf Gms. 
Sat Sol KNaC 4 H40 6 . 4 H 2 
Sat. Sol. per I00 Gms. Sat. Sol. 


O 


I.3IO 


53-33 


50 


0.908 


2.40 


10 


1.216 


41.60 


60 


0.878 


0.90 


20 


I.I24 


26.20 


70 


0.857 


0.30 


30 


1.034 


13-80 


80 


0.840 


O.o6 


4 6 


0.961 


6 


100 


0.789 


trace 



POTASSIUM DihydroxyTARTRATES K 2 C 4 H 4 Og.H 2 O and KHC 4 H A.H 2 0. 

100 gms. H 2 dissolve 2.66 gms. K^QHjOs.r^O at o. (Fenton, 1898.) 

100 gms. H 2 dissolve 2.70 gms. KHC4H 4 8 .H 2 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 Antimony TARTRATE C 2 H 2 (OH) 2 (COOK)(COOSbO).JH 2 0. 
loo gms. water dissolve 5.9 gms. salt at room temp. (Squire and Caines, 1905.) 
6. 9 " " " 2 5 . (S and S, 1903.) 

8 " " " 21. (Aschan, 1913.) 

11 95% HCOOH dissolve 82.7 gms. salt at 20.8. (Aschan, 1913.) 

" glycerol dissolve 5.5 gms. salt at 15.5. 

SOLUBILITY OF ANTIMONY POTASSIUM TARTRATE IN AQ. ALCOHOL 
SOLUTIONS AT 25. 

(Seidell, 1910.) 



Wt. Per cent 
CjHsOH in 

Solvent. 


Satst 


Gms. C 4 H 4 6 . 


Wt. Per cent 
QHsOH in 
Solvent. 


dnol 
Sat. Sol. 


Gms. CflfLOe. 
ico Gms. Sat. Sol. 


O 


1.052 


I ooGm,|at.Sol 


40 


0-935 


0.38 


S 


I.O25 


5-50 


So 


0.913 


0.23 


10 


1.007 


3-92 


60 


0.890 


O.I2 


2O 


0.980 


1.92 


70 


0.866 


O.O6 


30 


0.958 


0.84 


100 


0.788 


trace 



POTASSIUM SUCCINATE K g C 4 rt 4 4 . 3 H ? 

100 gms. Methyl Alcohol (CH 3 01I) sat. with anhydrous potassium succinate 
dissolve 3.16 gms. KG HO at 15 and 3.75 gms. at 66.6 (b.pt.). 
(Henstock, 1934.) 

POTASSIUM UKATE. KHC^H^O, 

O c 4 o 

SOLUBILITY OF POTASSIUM URATE IN WATER. (Barkan, 1924.) 
It was previously shown that sodium urate passes from a gelatin like colloidal 
form to a stable granular condition, and the author desired to learn if the potassium 
salt behaves likewise. Several different samples of potassium urate were prepared 
and used for solubility determinations. The solubility of each diminished with 
time of rotation. In general the diminution was from about 2.38 gms. per liter 
to 1.9 gms. per liter. The mean of all the determinations was : 

2.i3 gms. (== io.35 X io~ 3 gms. mols.) potassium urate per liter at 18: 
Several determinations of the solubility of the compound in the fresh colloidal 
form gave, as the Highest value, 6.67 gms. (= 32.4.io~ 3 gm. mols.) potassium 
urate per liter at 18. 



709 KALIUM K 



POTASSIUM CITRATE (CH,) a C(OH)(COOK) 8 .H>O. 
SOLUBILITY IN WATER. 

(Average results of Seidcll, 1910; Greenish and Smith, 1901; Kohlcr, 1897.) 
Cms. (CH 2 ) 2 C(OH)(COOK) 3 .H.,O per xoo Cms. 





Sat. Solution. 


Water. 


"* 


is 


6l.8 


l62 




20 


63.2 


172 




25 


64.5 


182 (</25 = 


1.518) 


30 


66 


194 





ioo gms. H 2 O dissolve 198.3 gms. (CH 2 ) 2 COH(COOK) 3 + 303.9 gms. cane 
sugar at 31.25. (Kohler, 1897.) 

SOLUBILITY OF POTASSIUM CITRATE IN AQUEOUS ETHYL ALCOHOL AT 25. 

(Seidell, 1910.) 

When potassium citrate is added to aqueous alcohol of certain concentrations 
the mixture separates into two liquid layers. A series of determinations made by 
adding an excess of the salt to 10-15 cc. portions of several aq. alcohol mixtures 
at 25 gave the following results. 



wt. % 

C 2 H 5 OH 
in Solvent. 




d&ot 
Sat. Solution. 


Wt. % 
C2H B OH in 
Sat. Solution. 


Gms. (CH,).,COJ 
(COOK)" : ;H 2 
per ioo Gms. 
Sat. Solution. 




(a 








9 


lb 


1.4920 


O 


60 " 




(a 






O.2 


32 


lb 


1.4930 


o 


6l.6 


f T 


(a 




65.1 


0.38 


5 1 


lb 






62.5 


70.2 


(a 
lb 


0.8366 


81" 


O.IO 

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, b lower, water rich layer. 

A series of determinations was also made by adding just enough potassium 
citrate to the alcohol solution to cause distinct clouding and then, after bringing 
to 25, titrating with the aqueous alcohol mixture to disappearance of the clouding. 
The results were plotted and the following interpolated values obtained. 

Wt p. Gms. (CH^jCOH- Wf Gms.CCH^COH- 

wt. % i r fr*r\f\v\ ix f\ Wt. % -f frt\r\v\ w r 

r> TT f\lT **25 01 t,L.Uv/iV;3.tl2vJ p TT f\ri <*2S OI t,L.VJUJx^a*lj^-' 

ii^nlvAnf Sat - Solution. per ioo Gms. ; n QI nf Sat - Solution, per ioo Gms. 

m Solvent - Sat. Sol. m Solvent - Sat. Sol. 

o 1.518 64.5 40 1.005 12.4 

5 1.400 52.5 50 0.943 5.6 

10 1.310 45.5 60 0.900 1.6 

20 1.177 51.5 70 0.868 0.4 

30 1.085 21.5 80 0.838 0.04 
In one determination at 15, made with alcohol of 59 Vol. per cent, 4.51 gms, 

(CH2)2COH(GOOK)3.H20 were required to just cause clouding. 

ioo gms. U.S. P. Glycerol (CH OHCHOHCH.OH) saturated with Potassium 
Citrate contain 28.2 gms. (CII 8 ) 2 C(OH) (COOK) 3 .1I 2 at 25. (Schnellbach 
and Rosin, 1931. ) 



C 5 H 



K KAIIUM 7* 

POTASSIUM PHENOLATES, CH E OK.*H a O, C 6 H 5 OK.3C 6 H 5 OH. 

EQUILIBRIUM IN THE SYSTEM POTASSIUM HYDROXIDE, PHENOL AND WATER AT 25. 

(Van Meurs, 1916.) 
Mole. per lOOmols. sat. sol. ^ Mols. per J 00 mols.sut. sol. 

C f H 5 OII. KOH. " Phase. C 6 H 5 OH. KOII. Phase. 

70.20 0.74 C 6 H 5 OH 20.93 17.13 G 6 H 3 OK.2H ; 

76 . 4o 4 * 3 22 . i 5 i 6 . 92 

60.16 7.28 C<jH 5 OK.3C 6 H 3 OH 14,95 i5.48 

51.27 8 -^2 8.84 1.5.39 

46.38 9.11 5.57 i5:i4 > 

33.79 1 1. 1 8 o-92 i6.o4 " 

29.70 17.13 o.o4 26.04 

3l.69 *9- 5 ))+C 6 H 5 OK.-2H 8 0.0 27.65 KOH.2H,0 

The two liquid layers which are formed at concentrations of K OH less than 
about 0.5 mol. % have the following compositions. 

Aqueous layr. Phenol layer. 



Mol. /o KOH. Mol. /o C,H S OH. Mol. "/ KOH. 

1.79 o.o 32.33 o.o 

2.48 0.19 21.60 0.37 

3.85 o.25 i5.85 o.45 

POTASSIUM PICKATB CHj(NOj)aOK. 

looocc. sat. solution of potassium picrate in water contain 5.o6gms. C fl H 2 (NO 2 )30K 
at 2O". (Mosor and Ritschol, 192^.) 

SOLUBILITY OF POTASSIUM PICRATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL, 
METHYL ALCOHOL AND OF ACETONE AT 25. (Fischer, 1914, 1918.) 

The composition of the aqueous alcohol and acetone mixtures, which served as 
solvents, was accurately controlled hy density determinations. Saturation was 
secured by constant agitation in a thermostat. The saturated solution was 
withdrawn by means of a graduated pipet and its dissolved picrate determined by 
evaporation and weighing the residue, or by a method of titration. The absolute 
alcohol was prepared by treatment with lime and distillation. 



Vol. 


Cms. 


Vol. 


Cms. 




Gms. 




Gins. 


per cent 


C 6 H S (NO S ),OK 


per cent 


C (i lI 2 (NO i ) a OK 


Vol. % 


C H a (N0 2 ) a OK. 


Vol. / Q 


C fi II 4 (i\0 2 i a O 


Cg Tig OH 


per 100 cc. 


c a n s on 


per 100 cc. 


CH a OH 


per toocc. 


Acetone 


per 100 cc. 


In solvent. . 


sat. sol. 


In solvent. 


sat. sol. 


In solvent. 


sal. sol. 


in solvent. 


sat. sol. 


0.0 (=11,0) 


o.645 


55 


0.598 


10 


0.542 


IO 


0.726 


10 


0.559 


60 


o.5;4 


20 


0.470 


20 


0.876 


i5 


0.475 


65 


0.546 


3o 


0.444 


3o 


I. l4o 


20 


o.45o 


70 


0.485 


4o 


. 4 22 


4o 


1. 155 


25 


0.453 


75 


0.410 


5o 


O.4II 


5o 


2. 106 


3o 


0.472 


80 


0.326 


60 


0.4lO 


60 


2.6i5 


35 


0.484 


85 


0.227 


70 


0.396 


70 


3.090 


4o 


0.533 


90 


0.174 


80 


0.332 


80 


3.34o 


45 


o.56o 


95 


O. IOO 


90 


0.254 


90 


3.o84 


5o 


0.582 


IOO 


0.184 (?) 


IOO 


o . 274 


IOO 


i .080 



Data for the solubility of potassium picrate in aqueous solutions 
of ethyl alcohol, methyl alcohol and of acetone at 25 are given by 
Fisher, 191/4. 



7" KAUUM K 



POTASSIUM *:ll i 

pjirti.iitiurM IN Titr. Svs-rrM I'or^nii'M HvnitnXf t*!-\ Hr.inuttiNoi. ANI> WATKII 

At' IffR (Wl MftllW, Bit* 



%, || tt 

iwtf t'imw ..-_,,.. M||| ^ 

HH.Ht t.o I. V H, *irt .; Hi. n ifi, ir" i- 4 H, <*k . ^ 

4i,Ho 1,-ifi - $1 . H it;, ,5!} 

%,!< I**, t I I . '| I -!'l,t 

<<t,H i It* *|i .. 0.7!* *lfi,i|i| - , ^ 

U,IM ift.lii - it,; ( I '**|,i|i 

*ti ^i i M o " . r/i 'i*i. $'i KOH - 

* t| l H 4 ' , -t 4 II, tiK { ,li s i* <>/il .Mf.HH KfM Kf< 

^ $* i , , t .4 * ,M. *, -M t u n. t ; i *i.r* 



l , *iiilwliit|i !f I*nl A 
41 j% w , <MAy, 



KtMUJj.oii*). 

1*4' WATKK. 



t t . 
CiiiH, Kt*|iyf 3 }wi toc> t!m. Hululifin 41 . i 44,4 44 46.6 

i;,H,i:tNih, 

>i*i riu 1 1 \ it }'fct .\i'itr M Mt^/>*Aii t \\.\titt. 



Hi , 

i:v 
$1$ ^ 
| MI , 



wi4 % ^^^, 4l */* I,* |*f,l, 
HOTAHHIUM lhili%i ft 



Hit 



K KALIUM 



712 



- SOLUBILITY OF POTASSIUM 
Meta Hydroxy Benzoate in Water. 



Cms. C 6 H 4 OH.COOK(m) Solid 

t 3 . per J oo gnus. sat. sol. Phase. 


- 2.41... 


12. 3 9 


Ice 


5.06... 


22.25 





- 8.5 9 ... 


3i.34 





19- 9 2 - 


49-39 





-4- IO.O 


69.04 


C 6 H 4 OH.COOK(m) 


33.5.... 


61.94 





95.0 


69.60 





136.8.... 


75.02 






SOLUBILITY OF POTASSIUM 
Para Hydroxy Benzoate in Water. 



Gras.C,H,OH.COOK(p) Solid 


t*. per 100 gins. at. 


sol. Phase.. 


1.43... 


8.04 


Ice 


3.24... 


15.55 





i5.8.... 


29-91 


(;>)C ri H 4 OW.COOK.:iIM> 


25.8.... 


35.5o 





43.o.... 


45.71 





64-4. 


56.70 





70.5.... 


59.34 





86.8.... 


63.oi 


(/>)C 6 H 4 OH.COOK 


129.5 


64.95 






POTASSIUM MANDELATE (Racemic) C.H-.CHOII.COOK 

o 

EQUILIBRIUM IN THB SYSTEM RACEMIC POTASSIUM MAN DEL AT 8, 
RACKMIC MANDBLIC ACID AND WATBR AT 25. 

(Posa and Morrison, 1973.) 



fas. per 100 9ns. sau - sol. 



C 8 H 



3 3 


47-3 


4.1 


45-2 


5.1 


37.2 


6.4 


33-3 


7.7 


30.8 


8.1 


29.7 


6.3 


27-7 


5-5 


24-7 


6.o 


23.1 


6.5 


19-5 


8.6 


16.2 


11.4 


14-5 


8.4 


16.5 


11.0 


15.6 


ii.6 


15-0 



Solid 
Phase 



fas, per loo ga*. aat. sol. 



Dc<c B H 7 o a gn s 



WB 


vw 


12.9 


13.7 1 


I/I .4 


12.3 


15.8 


11.2 


20.4 


9.8 


24.0 


9.4 


27.1 


0.8 


30.1 


8.5 


31-7 


8.3 


30.1 


7.7 


27-1 


6.7 


25.0 


5-5 


21.6 


3.8 


18.6 


1.1 


16.9 


0.0 



Solid 
Phase 



POTASSIUM MANDELATE 



(Laevo) C 6 H 5 CHOH.COOK 



EQUILIBRIUM IN THB SYSTEM (-) POTASSIUM MAHDBLATB 

(-) MANDBLIC ACID AND WATBR AT 25. 

(Ross, Morrison and John stone, 1937.) 



fas. per 100 



9.7 
34.4 
42.7 
39-8 



37.3 
27.2 



Solid 
Phase 



fas. per UK) BBS. aat. sol. 



C 



WT 

46.4 [K(C 8 H 7 3 gH 30.9 

38.5 " " 12.1 

10.5 



* K 8 3 ".I 
10.1 



17.7 

6.0 
3.2 

o.o 



Solid 
Phase 



7*3 



KALIUM K 



POTASSIUM PHTHALATE 



C e H 4 (COOK) g 



EQUILIBRIUM IN THK SYSTEM POTASSIUM PPTHALATB, PHTHALIC 
ACID AND WATER AT SEVERAL TEMPERATURES. 

(fitalth, 1931.) 



fas. per 100 9ns. sat. sol. 

VV 000 "^ C e H 4 fCOOK) % 

Results at o 



o.o 

o.io 

0.11 

0.19 

0.40 

1.06 

2.01 

1-55 
0.89 
0.30 

Results at 

o.o 

0.17 

0.27 

0.28 

0.36 

0.54 

0.77 

1.25 

3.07 

4.16 

3.93 

3-77 

2.6l 
1.72 
0.75 



Solid 
Phase 



Qns. per 100 



Solid 
Phase 



Results at 35 



60. 
60. 


4 


c i! 


,(COOK) 2 
+CJLICOOfl)<COOK) 


0. 
0. 




28 


78. 
75* 


5 
6 


48. 


89 


CJUCOO 


R1COOK 


0. 


27 


68. 


51 


33- 


02 


n 






0. 


33 


58. 


59 


20. 


43 


M 






0. 


38 


48. 


67 


8. 


33 


11 






0. 


51 


37- 


43 


4. 


01 


" 


+ i 


.4.4 


0. 


89 


27- 


07 


2. 


79 


1-4 


4 




1. 


28 


21. 


03 


2. 

1. 


12 
00 


C.H 


+ CJMCOOH). 

4 (co6nf g ? 


2. 

3- 


32 
23 


13. 

9- 


09 
76 






II 






5- 


10 


7- 


43 












5. 


70 


7- 


32 


25 










5. 


53 


6. 


64 












5. 


29 


6. 


35 


74. 


8 ( 


M! 4 


(COOK). 


4. 


74 


5. 


60 


74. 


7 




KC A 




2. 


38 


2. 


06 


60. 


97 


CJI 


4 (C(5 


OH) COOK 


0. 


98 


0. 





48. 


16 


n 














39. 


70 


" Results at 


60 




31- 


23 


" 














23- 


33 


" 






0. 





78. 


9 


16. 


65 


" 






0. 


40 


79- 





7. 


10 


" 






0. 


51 


64. 


17 


6. 


11 


11 


+ 1 


4.4 


0. 


80 


49. 


07 


5- 


41 


1.4 


4 




2. 


15 


29. 


66 


4* 
4. 


80 
12 


c l! 


* C.HJCOOH) 
4 <CoSHt, 


4. 

8. 


94 
50 


16. 

12. 


57 
59 


2. 


87 






14. 


14 


13- 


00 


1. 


47 


" 






7. 


68 


5- 


97 


0. 





M 






2. 


58 


0. 


00 



B H 4 (COOK) 2 

" + C ft H.(CDOlI)COOK 
8 H 4 (CO)S)COOK 



1.1.4 



.i^^CLlUCOOH). 

jucodtiL 



JT(COOKi 

"tcJuccfcmcooK 

.HjCOOTf)COOK 



1.4.4 = C 6 U 4 (COOK) J ,.4C e H 4 (COOH) J ,.4H ? 

The transition temperature above which this 1.4.4 double salt does not 
exist was found to be 36.68 and the composition of the saturated solu- 
tion at this temperature was 6.14 percent C fl H 4 (COOH) ? and 7.65 percent 



C,H JCOOK), 

04 c. 



POTASSIUM Hydrogen PHTHALATE KHC 8 H 4 8 . 

100 gms. sat. solution of potassium hydrogen phthalatc in water contain IO.23 gms. 
KH C 8 H 4 4 at 26, 12.67 gms. at 35 and 36.12 gms. al the b. pt. 

(Hendrixflon, 1920.) 



K KALIUM 714 

SOLUBILITY OF POTASSIUM PHTHALATE IN ALCOHOLS AT 20. 
(Handy and Hoyt, lo?7.) 

Qms. C 6 H 5 (COOK) ? 
Solvent per 100 cc solvent 

Ethyl Alcohol (absolute) 0.0161 

(95%) 0.0252 

100 vols. " " " + 10 Vols. CH 3 OH 0.0728 

Methyl Alcohol (CH,,OH) 0.792 
POTASSIUM PHENYL ACETATE CH 2 C 6 H 5 COOK 

Fusion-point data for mixtures of Potassium Phenyl acetate and 
Phenyl acetic acid, showing the formation of the compound CH^CgH 
CH^fij.COOH are given by Bakunin and Vitale, 1935. 

POTASSIUM Benzene SULFONATES 

SOLUBILITY OF EACH SEPARATELY IN WATER AT 25. 

(Elgersma, 19*).) 

Onus, anhydrous compound 
C nPOUnd *"" per 100 *.. H.O 

Potassium o Nitro benzene sulfonate K[N0 2 . 0^.50.,] 9.63 
% " ' ..... " 3-04 

" " ;; " " .HO 5.95 

" o Diuitro " '' K[(NO ) .C -H.-SOll 4.70 

c H "2 Nitro 4 Chlor " KCNO ? fCgH 3 ClSCg 0.87 

8 " 2 !', f !! !! !! " ' ^^ 

3 " 6 " " " 2.83 

" 2 " 4 Brom KLNO p .C 6 H 3 Bp SOJ 1.68 

100 gms. sat. solution of Potassium m chloro benzene Sulfonate in water 
contain 3.12 gms. m C^CISO K at 18 and approximately 45.0 gms. at 98. 

100 gms. sat. solution of Potassium 2 chloro benzene sulfonate in water 
contain 0.73 g"- 2 C 6 H 4 C1S0 3 K at 18 and approximately 40.0 gms. at 98. 

(Bellinger, 1928.) 

100 gms. Methyl Alcohol sat. with Potassium Benzene Sulfonate contain 
2.67 gms. C 6 H S S0 3 K at 15 and 9.67 gms. at 66.1 (b.pt.). (Henstock, 

100 gms. acetone dissolve 0.12 gin. C fl H 5 S0 3 K at 15. (Henstock, 

POTASSIUM Anthraquinone SULFONATES 

SOLUBILITY OF EACH SEPARATELY IN WATER. 

(Flerz-David. Krebsen and Anderau. 1927.) 

c o 0^* 

-Potassium Anthraquinone 1.5 Disulfonate KJL A0 (SO ) 18 07 

n n H ,i ^ 14 e p 3 2 u * ' 

100 3.5 

. I ';, 8 I K C i4 H e f ts 8 'p- aH 8 ^ 0.65 

" 100 2.2 

i ,-, 6 ;; VuWSfy^iiH.o 18 ,. s 

100 1^.3 
V 1' K C i4 H 'S0 8 >8-a 8 18 4.3 

C 1 HOaSO,.aH "a S o'. 
* 



8 

1.6 " K HOC1SO, ^8 o.l? 

1.7 " KC^H 8 8 O^ClSO^.iiH 2 18 2.0 



7i5 KALiUM K 

POTASSIUM Naphthylamine DiSULFONATES, 2.6.8 and 2.5.7 C 10 H 5 . 

(NH,)(S0 3 K) 2 . 

POTASSIUM Acid Naphthylamine Di SULFONATES, 2.6.8 and 1.5.7 
C 1() H,(NH 2 )(SO a K)(SO :j H). 

SOLUBILITY OF EACH SEPARATELY IN WATER AT Jo. (Braunschweig, 1922.) 

Gins. cmpd. 
Compound. por 100 gms. sat. sol. 

2.6.8 Potassium naphthylamine Disulfonate 5i.6 

2.6.7 68.9 

2.6.8 Acid 2.47 

2.5.7 w w }> 2 -58 



POTASSIUM SULFONATES 

SOLUBILITY OP EACH SEPARATELY IN WATER. 

Ctas. Anhydrous 
Compound t Qnpd. per 100 Authority 

Potassium: * H j> 

Naphthalene Monosiilfonate.iH 25 8.48* (Witt, 1915.) 

11 -2- Sulfonate 16.5 8.12 (Ephraim & Pfister, 1925.) 

" 1.4. Chloro Sulfonate 18 0.73 (Ferrero and Bolliger, 1928.) 

" 1.5 " " 18 3.12 " " " " 

Naphthylamine 2.^.7 Sulfonate 20 29.3 (Frisch, 1930.) p T 

" " 80 66.3 " " 10 

2 Phenanthrene Monosulfonate.iH 20 0.273 (Sandgtuist, 1912.) 

3 " " .ol! p 20 0.342 

10 " " .iH ? 20 0.84 " " 

" 10 Chloro 3 or 6 Sulfonate 20 0.248 " ! ' 17 

Guaiacol Sulfonate (Thiocol) 15-20 16.6 (S-iuire & Caines, 1905.) 

d * = 1.029 

ioocc.9ovol.% alcohol dissolve 0.25 gm. thiocol at 13-20. (Squire & 

Caines, 1905.) 



POTASSIUM Cymene SULFONATE KCH 3 C fl H 4 CH 2 .CH g CH 2 .S0 3 

SOLUBILITY OF POTASSIUM CYMBNI SULPOHATE IN WATER. 

(Hausllc^ 1935.) 

Cta. Mola. Sulfonatt <k. Mols. ailfonate 

c per 100 918. H^3 fc Pr 100 gns. H g O 

2.5 0.025 45 0.250 

15.0 0.056 68 0.523 

31.0 0.133 90 0.994 



K KALIUM 



716 



POTASSIUM CAMPHOEAT1S 

SOLUBILITY IN AQUEOUS SOLUTIONS OF d CAMPHORIC ACID AT 13.5-16 AND 

VICE VERSA, 

(Jungfidsch and Umdrieu, 1914.) 

Cms, per goo Gms. Sat. Sol. 



Gras. per 100 Gms. Sat. Sol. 


QH4(COOH) 3 . 


CuHuQiKi. 


O 


66.65 


0.90 


69.69 


I 


69 


1. 10 


66.79 


0.90 


66.65 


1.50 


62.37 


2.60 


59-34 


3.20 


58.37 


3.20 


58.09 


3.20 


52.71 


3.20 


48.43 


2.80 


47.88 


2.80 


42.36 


3 


3S-&> 


2.85 


34-77 



Solid Phase. 



CioHi 4 O 4 K : m Dipotasiium rf caiphofit. 
jj CiftHiAK - Mon0potMium^mphom 



2,90 


32,84 


3.20 


^9-39 


3.30 


28.56 


3.20 


27,32 


3.20 


22.77 


3.10 


21.66 


2.90 


12.97 


2.90 


11.73 


3.10 


11.59 


2.90 


9.66 


2.80 


8.14 


2,50 


6.76 


2.30 


6.07 


2 


4- 55 


0.621 


o 



Solid Phase. 



MwjlA*ilttm i dii amphorute. 



POTASSroM HELIANTHATB KC. l4 H i4 N a SO a ,all s O. 
1000 cc. H t O dissolve 4-368 gms. K C u H u N t SO t .i H ft at 



id JDthn, 1018.) 



POTASSIUM LI0NOCBBATB. C 1S H 

100 gms. aq. 91.53 wt. pet cent ethyl alcohol dissolve 0.1 53 gm. potassium 
lignocorate at ^5 aad the solution has d ** o.8og3^. (Thom ana Vw, i$.j 



POTASSIUM Salt of OABYOPHYLLXN Kf :,,!! t ,0t. i/,H,O. 
100 gins. Ethyl alcohol dissolve 2,78 gm*. tf tin* suit at 10**. 
Methyl alcohol .-{o.o 



POTASSIUM Salts of 



717 



KALIUM K 



EQUILIBRIUM IN THE SYSTEM POTASSIUM HYDROXIDE, PHENOLPHTHALEIN 

AND WATER AT 25. ( Bassott and Bagnall, 1924. ) 

NOTE. Saturation was obtained by constant rotation for not less than 3 days 
of mixtures of phenolphthalein and aqueous potassium hydroxide solutions of 
various strengths. Such concentrations were chosen that a liquid and a solid 
phase was obtained in all cases. Both the saturated solution and the solid phase 
was analyzed. No solid colored salt was obtained. The results are expressed in 
terms of phenolphthalein anhydride (C 20 H 12 8 ) potassium, oxide (K 2 0) and water. 



Gms. per 100 gms. 
sat, sol. 


Solid Phnsc. 


Gms. per 100 gms. 
sat, sot. 

'TtToT^^ni^O^ Solid Phase. 


Cms. per 
sat. 


100 gms. 
sol. 

Tl^tflTo? Solid Phase. 


4 .'96 


i3.86 


P 


17 


.3i 


3 9 . 


or P.K 2 .8 


29* 


.5o 


2.03 P.K 3 .8 


7-49 


*4 


.20 







17 


. i5 


44- 


90 P.K 3 .4 


*4 


74 


10.70 P.K 3 .7 


8.25 


25 


.06 


P. 


KJ5 


16 


.5o 


4o. 


74 


3o 


.90 


1.14 


8.97 


27 


. 7 5 







16 


98 


3 9 . 


22 


3l 


.65 


o . 76 


12.43 


38 


74 




)> 


16 


.60 


3 7 . 


06 


34 


.32 


0.06 


1 3. 22 


39 


.91 







17 


.72 


33. 


*4 P.K 3 . 9 


36 


.24 


)) 


11.26 


33 


.60 


P, 


K.4 


19 


.84 


27. 


47 


39 


. IO 


- 


14. *4 


4i 


.69 







21 


.5 7 


22. 


ii 


39 


.57 


P.K 3 .6 


i3.f9 


4o 


.34 


P. 


K.3 


17 


.80 


35. 


67 


4* 


.14 


- 


i5.u 


44 


.3i 







19 


.68 


3o. 


90 


a'3 


:62 


P.K,. 5 


15.77 


45 


:/C> 


P.K 2 .io 


22 


. :>. I 


"9* 


47 P.K 3 .8 


45 


.60 


- 


15.88 


44 


.66 







24 


74 


10. 


70 


46 


-49 


- P.Kj.l 


16.44 


43 


.5o 


P. 


K-.o, 


25 


.64 


8. 




47 


.44 


)) 


15.92 


43 


.80 


P. 


K 2 ".8 


28 


.27 


3. 


10 


45 


.44 


- 4-KOII.-JH a < 


16.62 


42 


.62 







28 


.98 


2. 


69 









P = Phenolphtalein; P.K. 5, P. K.4, P. K.3 = Mono potassium salt : 

. 311,0; 



C 14 H 



., 4 
P.Kj.io, P.Kj.g, P.K 2 .8 = Di potassium salt : 



P.K n .4, P.K 3 .9, .8, etc. = Tri potassium salt : 



, 8H,0, etc. 



POTASSIUM LAURATE 



, rt 

10 



COOK 



100 gms. Water dissolve approx. 70.0 gms. CH (CH ) COOK at 25. 
11 " Benzene " " 0.005 " " " 

Results are also given for the extraction of lauric acid from aqueous 
solutions of potassium laurate and of sodium laurate by means of benzene. 
(McRain and Eaton, 1928. ) 

The phase rule diagrams for equilibrium in the system potassium laurate 
lauric acid + water, at temperatures between 100 and 370 are given 
by McRain and Field, 1933. Due to high viscosity, even at 90, months 
may be required for the separation of the liquid phases. The existence 
of acid soaps is demonstrated by the separation of crystalline sediments 
from dilute solutions of soluble soap such as potassium laurate. At 
370 the three components are almost but not quite soluble in all pro- 
portions. 



K KALIUM 7i 

POTASSIUM STEARATE CH n fCH^ Jg COOK. 

too gms.aq. alcohol of di* = o.8o<)35 (=91.53 wt.% C 2 H 5 OH) dissolve 0.633 gm. 
CH 3 (CH 2 ) M CO OK at i& ( Th m * "* Vu, loan, i 

SOLUBILITY op POTASSIUM STBARATTS AKD OF POTASSIUM PALNITATE 
IN AQUEOUS ETHYL ALCOHOL AT 18. 

(Schtrlnga, 193?.) 
Potassium Stearate Potassium Palmitate 



Qns. Cj^OH per Ctas. CH^CHjj) ta COQK taft. C^gOH Ptr dan. CH 3 (CH ? ) ^COOK 

100 88. Solvent pr 100 gas. sat. sol. 100 *p. Solvent ptr 100 ^}nu. &t. ol. 

/I9 <|.4 49 45*0* 

66 2.6 66 19.0 

79.5 1.8 79-5 6.5 

96 0.62 96 1.4 

* This result uncertain on account of the colloidal character of the 
Solution. 

POTASSIUM OLEATE C 8 H |7 CH : CII(CH,)7CO()K. 

100 gms. of aq. 91. 53 wt. per cent C a H 8 OH dissolve 41.1 gins. C 18 H 3I O t K 
at 25 and the saturated solution has d -- o.Bo(j35. (ThomnH ami YU, i9->3. / 

Results are given by McBain and Stewart, 1933, for ^uilibrium in the 
System Potassium Oleate + Oleic Acid, determined by observing the tem- 
perature of disappearance of the last crystal upon heating, and the 
first appearance of turbidity upon cooliag known mixtures of the two 
components contained in sealed evacuated tubes. An acid soap of the 
composition, C e H l7 CH:CH(CH J ,) 7 COOK.C B H l7 CH:CH(CH 1 ) 7 COOM exists below its 
transition temp, of 47 
POTASSIUM CYANIDE KCN. 

100 gms. H*0 dissolve 122.2 gms. KCN, or 100 gms, KU. solution contain 55 
gms. KCN at 103.3. ^ ^ (Griffith*.) 

100 gins. abs. ethyl alcohol dissolve 0.87 gm, KCN at 19.5. 
100 gms. abs. methyl alcohol dissolve 4.91 gm. KCN at 19.5. (tie Bruyn, 1891.) 
loo gms. glycerol dissolve 325 gms. KCN at !55 (Owemlowiki, 1907.) 

100 gms. hydroxylamine dissolve 41 gms. KC"N at xy.S' . (<1 Bruyn, iB^a.) 

100 gms. liquid auumonia (NH^) dissolve ^.55 gws KCN AI -^3,9 iti the 
density of the sat. solution is 0.7034, (Johnson and Kruiiboliz, 1933.) 
100 gtns. liquid sulfur dioxide (SO,,) dissolve 0.017 g m * KCN At o , 

Uander and Ruppolt, 1937.) 

F.-pt. data for KCN + KG, KCN + NaCN, KCN -f AgCN r KCN + Cm 

(CN)i and for KCN 4- Zn(CN) are given by Truthe (1912). 

POTASSIUM CHROMOCYANIDE KiCr(CN). 

100 gms. H S dissolve 32,33 gms. KaCr(CN)e at 20. 

(Moitn, 1885; ClurbteoMa, 1885.) 

POTASSIUM CHKOMITfflOCYAHATl KiCr(SCN)4lW). 

roc gms. HgO dissolve 139 gms. salt. (Kaii, 1864-5.) 



7i9 KALIUM K 

SOLUBILITY OF POTASSIUM CYANIDE IN AQUEOUS SOLUTIONS OF NICKEL CYANIDE 
AT $5 AND VICE VERSA. (Corbet, 1926.) 

Note. In the case of this and the following experiments by Bassett 
aad Corbet the authors prepared the KCN from pure double salts in order 
to obtain it free of KOH. In order to prevent oxidation an atmosphere 
of coal gas previously passed through solutions of lead acetate and 
sodium hydroxide was maintained in the bottles. Both the liquid and 
the solid phases were analyzed. 

Gms. Gms. 

per 100 gms. sat. sol. por 100 gms. sat, sol. 

KCN. NI(CN) 9 . Phase. KCN. Nt(CNJ t . Phase. 

39.85 i. oo KCN 23.97 10.82 KjNi(CN) 4 .H a O 

38.79 1.88 23.14 io.34 

37.64 4.69 16.82 14.29 

*4i.n 6.56 16.82 i3.o.4 -hNi(CN)s 

39.09 5.95 KCN-r-KiNi(CN; 4 .HiO io.58 g.i3 Ni<CN) 2 

30.94 7.46 K 9 Ni(CN) 4 .H 2 0.28 o.23 

"Unstable equilibrium. 

SOLUBILITY OF POTASSIUM CYANIDE IN AQUEOUS SOLUTIONS 
OF POTASSIUM HYDROXIDE AT 25. (Basset and Corbet, 1024.) { 

Cms. per 100 gms. sal. sol. Cms. per ioo gms. sat, sol. 

"KCN"-H KOH. 
42 . 1 1 
42.54 
42.68 

Mn terms of KCN. Those results show that KOH decreases the solubility of KCN in water. 
Hence accurate result* require that KCN free of KOH must be used for solubility determinations. 



SOLUBILITY OF POTASSIUM CYANIDE IN AQUEOUS SOLUTIONS OF THALLIUM CYANIDJE 

AT 25 AND VICE VERSA. (Bassett and Corbet, 1924.) 

Gms. per lOO gms. sot, .sol. . iiiu^poi' 100 gms. sat, nol. 

KCN. TICN. 8Hd Phuse KCN. T1CN. Solid Phasr. 

41.7 o.o KGN 34.36 4.90 T1GN 

4o.83 0.71 M, 35.09 4.96 

39.76 i.65 *3i.25 4-46 

37.0 3.17 H-KTl(CN)* 3o.2i 5.00 

37.5 3.n KT1(CN) 4 28.07 4.47 

36.47 4- l(i w 21.00 4.36 

36.52 4.12 > i4.75 5.46 w 

35.93 5.78 9.12 7.17 > 

36.oo 4.99 T1CN o.5i 16.20 

35.27 4.98 0.34 16.12 

34.45 4.91 .. o.oo 16.61 



KCN. 


KOH*. 


KCN + KOH. 


KCN. 


KOH*. 


41-56 


O. I I 


41.67 


34-7* 


7-39 


41.67 


0.69 


42.36 


33.58 


8.96 


38.92 


3.3 


42.22 


26.39 


16.29 



K KALIUM 720 

SOLUBILITY OF POTASSIUM CYANIDE i 
AT $5 AND VICE VERSA. (< 

6ms. pr 100 gms. sat. sot. < ; - PT "X Km*, sal. sol. 



SOLUBILITY OF POTASSIUM CYANIDE IN AQUEOUS SOLUTIONS OF ZINC CYANII 
AT $5 AND VICE VERSA. (Corbet, 1920.) 



KCN. Zn(CXi,. Solid Ph*st\ Kl'.X. ZnittK. Solid Mi MC . 

41.7 o.oo KCN i8.'i'>. 0.47 

4 1. 1 5 trace -hK 2 Zn(C\U 14.17 i.5o 

39. of trace K 5 Zu(('l\)v 7.<>"> "^7'J 

37.1;") o.r>. <<>4 5.86 

34-4<> 0.17 6.77 6.97 

// > i *t *i M 

cta.65 0.20 ** >.oi .>..> 

a3.56 0.67 a.5< 2.:*o 



POTASSIUM ZINC CYANIDE K 2 Zn(CN)4. 

100 cc. HaO dissolve n gras. K 2 Zn(CN)4 at 20. (Shtrwood, 1903.) 

POTASSIUM FERRICYANTDE K 3 Pe(CN) e 

SOLDBILITY OF POTASSIUM PXFRXCYANIDB IN 

CN 



t 


a of a 


(friend and Italrlos, 

as. K-Pe(CN),, per 100 g^o. 

,,,, ,,,fi .- .^yv-t _ ..._.... . _ v 


a or a 


ws. K n ft(CN> 


, ptr 100 i 


0.1 


sac. sol.' 


a&t. aol. 


30.24 


^ " MC. OX. ^ ll*t:'lol. 

29.8 36.65 


~~?~" 

'S3- 02 


14.. 7 





25-49 


34.21 


33-1 


1.2045 


~ 





7.8 


1.1567 


26.96 


36.95 


39-9 


1.2115 


37. aa 


59,27 


15-7 


1.1738 


30.35 


43.58 


49-0 





39- 13 


64*25 


18.7 





30.96 


44.85 


56.25 


- 


40.41 


67.80 


22.1 


1.1872 


32.08 


47.22 


58.0 


1.2269 


41.10 


69.78 


2S.O 





32.80 


<i8.8o 


8l.O 





44.70 


80.82 


26.3 


1.1928 


33.66 


50.74 


99.0 





47.60 


90.83 



The solid phase is K" Pe|CN) 6 in all cases and there is no indication 
of a break in the solubility or density curve* The saturated solutions 
were prepared by continuous agitation for 6 hours and analyzed by a 
gravimetric determination of the Fe. The previous determinations of 
Wallace, 1855; Schiff, 1860 and Grube, 1916 are slightly lower than the 
present results. 

One liter sat. sol. in 0.4687 n KOH;contein8j342.7 gm KPe(CN )* at 25*, (Grab* 1914.) 

0.9628 " " 302.3 <4 " 

11 " 1.949 4 * " 215.1 * 4 " *' " 

100 cc. anKy. hydrazine dissolve 2 gm. KFe(CN)i at room temp. 

(Welsh and Brodtiwo, 191$.) 



100 gros, methyl alcohol dissolve 0.31 P' Potassium ferricy^nide 
the b. pt. (66), (Henstock, 1934.) 



at 



721 KALIUM K 

POTASSIUM FERROCYANIDE 



SOLUBILITY op POTASSIUM FERROCYANIDB IN WATER. 

C Harkins & Pearce, 1916; Fabris, 1921, 1931, 1932; Vallance, 1922; 
Farrow, 1926; Bovalini and Fabris, 1933.) 

The results of the above named investigators were plotted on cross 
section paper and from the average curve drawn through them the follow- 
ing values were read. 

Q d of Qtos. K 4 Fe(CH) e Solid Q d of Gtas. K 4 Fe(CN) fl Solid 

1 sac. sol. oer 100 0ns. sac. sol. Phase c sac. sol. per 100 gras. sac. sol Phase 

-0.24 1.25 Tee 50 1.2350 32.6 K 4 Fe(CN) 6 .3Hp 

-0.62 ^.o " 65 1.2635 36.8 " 

-1.09 8.0 " 70 38.2 " 

-1.6 tec.- 11.6 "^K^etCNig-So 1.2854 40.1 " 

38 ? 87.3 41-34 ."* K FeCN') 6 

o 12.5 K 4 Fe(CN) e .3HjP 94 41.99 K 4 Fe(Cl5) 6 

5 15.0 M 99.6 42.63 " 

10 17.36 " 104.1 44-77 " 

15 19.3 " 88.3 41-68* K 4 Fe(CN) 6 .3H, 8 

20 22.0 " 90 42.24* " 

2$ 1.1731 24.0 " 94 43.91* " 

30 26.0 " 95-8 44.74* " 

35 1.2018 27.8 " 

CN 

* Metastable 
SOLUBILITY OF POTASSIUM FKRROCYANIDE IN WATER AT TEMPERATURES UP TO 25. 

(Vallance, 19??.) 

The author first compared the available methods of estimating potassium 
ferrocyanide in solution and selected as most accurate, the method based 
upon decomposition of the dry salt with cone. H p S0 4 and a little HNO,, 
and finally dissolving in cone. HC1, diluting and precipitating the Fe 
with ammonia, filtering, igniting and weighing. The very careful solu- 
bility determinations give a curve in whrch there is a break at about 
18. No difference in the crystal fo'rm or composition, K 4 Fe(CN) e .3HJ) 
of the solid phase, above and below this point could be detected. Trie 
density curve of the saturated solutions also shows a slight change in 
direction above 17. The dilatometric method shows a transition point 



d of Ctas. K 4 FefCN) f per Q d of Ctas. K 4 Fe(CN) fl per 

1 sac. sol. 100 <pa sue. sol. l sac. sol. loo 0ns. sac. sol. 

1$ 1.1378 19.S2 19.0 1.1505 21.08 

16 1.1415 20.00 20.0 1.1543 21.9 

17 1.1455 21.00 22.5 I.l6l5 22.7 
17.7 1.1471 25.6* 25-0 1.1701 23.97 

SOLUBILITY OF POTASSIUM FERROCYANIDE IN Aq. POTASSIUM HYDROXIDE 
SOLUTIONS AT 25 (Grube, 1914.) 

Gmi. Gms, 

Solvent K<F<KCN) fl . 3 H 2 Solid ^ K<Fe(CN) fl . 3 H 2 Solid 

^wivtui,. r ^ r r/vu% ^ Pha OVMVt.Hl. ^^ JQQQ C ^ PhaSC. 



Sat. Sol. Sat. Sol. 

0. 09984 wKOH 308.5 K 4 Fe(CN) fl .3H 2 0.9415 11 KOH 184.8 K 4 Fe(CN) a .3H a O 

0.2496 " 283.5 4< 1-395 u I3 2 -i 

0.4963 " 247.1 1.883 " 86.12 

0.7036 " 217.4 



K 



CN 



KAL1UM 722 

SOLUBILITY OF MIXTURES OF POTASSIUM FERROCYANIDK AND FERRICYANIDE 
IN WATER AND IN AQ. POTASSIUM HYDROXIDE SOLUTIONS AT 25, (Grube, i 

Cms. per 1000 cc. Sat. Solution. 
Solvent ' XFe^-N),. ' K 4 Ke<eN): 

Water 338.1 79 - 02 

o.4687ttKOH 309 66.64 

0.9628 " 275.3 55.19 

1.949 " 200.8 35.95 

SOLUBILITY OF POTASSIUM FERROCYANIDE IN AQUEOUS SOLUTIONS OF 
SODIUM FERROCYANIDE AT 25 AND VICE VERSA. (Hurkios md Pearce, 1916.) 

Mols. per loop Gms. H 4 0. iLFefCNT). <*aA f Moi8.pcrioooGm._H|O. * mi " 



JNa 4 Ke(CN). K4Fe(CN) 6 .P r *|o Cfmi - 


Sat. Sol. i 


41*104)1 


,. NitFeCCN) 


9 JWIGOO 




Sat. Sol. 







0. 


89459 


329- 


5 


I.00o8l 


o 


0.6818 


205. 


^S 


1-0505 


0. 


05072 


0. 


88272 


325- 


I 


1.0990 


0.1327 


0.7056 


214, 


47 


1,0199 


0. 


06633 


o. 


88544 


326 




I . 10039 


0.1789 


0.7213 


2. 1C). 


23 


1.0702 


0. 


12306 


0. 


88088 


324- 


4 


1.09350 


0.2115 


0.7253 


22O, 


44 


x. 1006 


0. 


25972 


0. 


89116 


328. 


3 


I. 12796 


o. 2722 


0.7610 


231. 


29 


1,1113 


0. 


4900 


o. 


91600 


337- 


4 


1.17241 


0.3532 


0,7814 


2^7. 


40 


1.1243 


O. 


87034 


0. 


99000 


364. 


6 


I. I97OO 


0.5850 


0.8652 


262. 


07 


1.1567 


0. 


9100*0 


I. 


OI2OO 


372. 


3 


I.2II9O 


o,6m 


0,8712 


264 , 


70 


1.1581 


0. 


95879 


I. 


05177 


387- 


S 


1.22673 


o . 6904 


0.8084 


273, 


05 


x . 1830 


I. 


043 8 


I. 


"59 


411 




1-25789 


1.0578 


0.0588 


301- 


40 


1,1267 


EQUILIBRIUM IN THI SYSTEM 


POTASSiriM FftRXOCYANIDB. 


POTASSIUM SWLFATI AM 


WATER. 








(Bovallnl nd FaDfla, 1'j^, ) 


t 


Ose. per tOO Solid 


Una. ptr tOO tioUd 




pna. sat. sol. Ph&M pit. *tt* ttju f%ti 




*' 


^T-^~-~ 


X)p * 


t4 








^fi?*j 








-1. 


6 


11. 


58 o 


.0 Ice + 


K. 3 


65 


38,8i 


0,0 


K. 3 




-2. 


05 


9. 


07 4 


.62 


M 


" * K f SO 


n 


33645 


3-31$ 




* K f SO 







9- 


80 4 


83 




n it 


H 


0.0 


l6.0 


ICSi 


D t 4 







12. 


48 


.0 




M 


74 


18.75 


0,0 


V 









0. 


o 6 


.82 K 


? SO. 




n 


36.30 


1-295 




* K SO 


30 




25- 


94 


.0 K 


3 




H 


0.0 


16.93 


M 


' 4 


it 




24. 


17 


.902 


M 




85 


40.72 


0.0 


K ; 3 


i 


if 




22. 


97 2 


.231 


n 




H 


3B.7IS 


3*975 




*" ^^ 


H 




22. 


23 3 


.902 


H 4. 


K*S0 4 


M 


0.0 


l8*U 


K. 


D 4 4 


II 




16. 


45 5 


S3$K 


,S0 4 




86.3 


39-03 


a.Bd 


KI 3 


J K.Fe 


II 




11. 


08 7 


.126 














NL* K so 


II 




8. 


54 7 


.818 


II 




90 


41.3S 


0,0 


K P 


efCHj' 


M 




5- 


01 9 


59 


II 




H 


40.14 


1.030 


H 




" 




3* 


03 10 


.205 


II 




H 


39.75 


1.4x0 


H 




" 




0. 


11 


53 


11 




It 


39*30 


3.770 


H 




40 




29. 


28 o 


.0 K 


.3 







39.*6s 


3831 


W 


* K SO 


M 




28. 


58 1 


,288 


II 




tf 


33. U 


4 30 


M 


4 ' 4 


" 




27. 


50 2 


.468 


II 




It 


30.36 


$.a6 


H 




II 




25. 


66 3 


.982 


t 4, 


K..HO 





17*30 


9.93 


H 




II 




19. 


63 5 


495K 


!S0 4 




n 


14.67 


11*09 


M 




" 




15- 


21 7 


.031 


H 




H 


5-46 


1$<U 


** 




" 




10. 


36 8 


557 


n 




H 


0.0 


18-60 


ft 




" 




8. 


56 8 


930 


n 


104. 


ifb.pU 


44.77 


0,0 


*\ . r ' 




II 




5. 


88 10 


. ill 


H 


10 4 


3 " 


39.3$6 


1 * 344 


1* 


"V'K i) 


" 




3* 


03 11 


.306 


It 


101. 


4 





*9.$C 


K 3 


D 4 






0. 


12 


90 


H 















K. 3 = 



7*3 

SOLUBILITY OF POTASSIUM FKRROCYANIDTI IN AQUEOUS 
SOLUTIONS or AMMONIA AT 18. 

(Tettamanai, 1333.) 



KALIUM 



per 100 jns. aat. aoi. 



0.0 


21.21 


4.51 
9.13 

11.86 


11.20 
5.65 
3-76 


15.19 
16.79 
18.11 


2.24 

1.53 
1.16 



Solid 
Phase 



Gtas. per 100 gna. aat. sol. 



K 4 Fe(CN) 6 . 3 H 2 



' NH * 


*4*(> fl * 


20.60 


0.872 K 


22.37 
23.62 


0.750 
0.6/is 


25.05 
26.95 


0.497 
0.427 


34.09 


0.157 



Solid 
Phase 



K 4 Fe(CN) 6 .3H 2 



100 gms. Methyl Alcohol dissolve 0.90 gm. Potassium ferrocyanide at 
the b. pt. (66). (Henstock, 1934.) 

EQUILIBRIUM IN THE SYSTEM POTASSIUM FBRROCYANIDK, TERTIARY 
BUTYL ALCOHOL AND WATBR AT 25. 

(Qlnnlnga, Herring and Webb, 1955.) 

The composition of the homogeneous mixture (plait point) of this system 
was found to be 

4.3 percent K 3 ?e(CN) 6 + 38.0 percent ter. (CH 3 ) 3 COH + 57.7 percent H g O 
The original results for the remaining points on the binodal curve are 
not given but only the values of a series of arbitrary constants calcu- 
lated from them by means of empirical equations. 

SOLUBILITY OP POTASSIUM FEKROCYANIDE IN 
AQUEOUS SOLUTIONS OF ETHYL ALCOHOL AT 20. 

da Kadtt arid Beratjo, 19?9.) 



Vol. Percent 


Gta8. K 4 Pe(Ol)L. per 


Ji OH in Solvent 


100 ew. aat. sol. 


( H^O 


) 22.01 


5 


16.40 


10 


10.47 


15 


6.6l 


20 


3.905 


25 


2.394 


30 


1.420 


35 


0.789 




0.565 


POTASSIUM 


CYANATE KCNO. 



Vol. Percent 
in Solvent 



15 
50 
55 
60 

65 
70 

75 
80 

85 



SOLUBILITY IN ALCOHOLIC MIXTURES. 

(Erdmann, 1893.) 
Solvent. 



Ota a. 

100 0n*. sat. so 1. 



0.352 
0.229 
0.143 
0.094 
0.057 
0.053 
0.039 
0.025 
none 



Cms. KCNO 

per Liter Solvent 

at b.-pt. 



80 per cent Alcohol + 20 per cent Water 

80 per cent Alcohol + 20 per cent Methyl Alcohol 76 

80 per cent Alcohol + 10 per cent Acetone 82 

ioo gins, alcohol of d ri r- 0.799 dissolve 0.16 gm. KCNO at o" and o.53 gm. at b. pt. 
80 %> concentration dissolve 1.9 gms.KGNO at oand 6. a gms. ath.pt 

benzene dissolve o.iH gm. KCNO all), pt. (Cranston and Livingstone, 1926.) 
ioo gms. liquid Ammonia, NH 3 , dissolve 1.7 gm. KCNO at 25. 
" " " 1.02 " " " " 

(Hunt, 1932.) 



cc. 



KALIUM '*+ 

POTASSIUM Platino CYANIDE K.I'U CiN h.1!I,O, 
SOLUBILITY or POTAJHUVM PLATJNU CVANUH-; IN WATKN. riWvy nd Jolly, 19 
Saturation secured i>y constant stirring in a thermostat. 

cwn.K.HiOi't . t t7*'i k|P l' < i?ii 

o.i ii . Go K,rt':K v , 4 ** tj > . ,| 1 

9.8..... 19.76 %.!.... IN|. 

i4.4....- 6.W J*-i" i- 

'4 "JK n tit HnlHii'^5. .'ili.tl M, i. , $ **", t 

lj.j)*"I' W| ' * * ,* ,* 

i7.4 4J> .- U^.O'A " <r .... tlt,) 

20.05.... 3'i.HlJ " 7-i- 11 * ^ ! C.*> 

a5!o////. 4 / i^l ' HJ.'tt!!!! t;H/i ' V' 

35 . o . 0i . t (J ** H ^ ,.*,,,, i H .J *> 

3c)]7">.... 7H.*>,"J <.*.,,, -nM.il 

The transition temperature* (tr. |t.) w*r0 itrlentiinrtl hy thr (ittttttisnrtric mcth 



POTASSItlM TlirOfYANATK 

CNS SotOiXLiTY 0r Pr>TAt8XitN TMZOCVAMATH ti* VATW. 



(Up to 35% Rudorff* iS% *B7a; Fooif, 

Occleshaw* 1931. Ai the higher 



The deteini nations of Kracek wer^ &y ftfestfift| the temper At ure 

of dls&ppear&nce of the l*t cr|it*I in Pixi^rct of * II contained 

in sealed tabes. A poiyworpliic invemion of Kt*N'S nccum At Iti0*6 , 



hence the solttblilty curve h** & At 



KOfl per 100 gut, ,, **. HW f#r lf ipw. 

HUM lf ' "^ ' A , ,|,v 

-6,$ ao.o 16.7 ^* 0^o *7*.6 H?iifi Kt*N$ II 

"9S5 30.0 as* I ** 108* fttJ**i SS.fi M 

-31.2 101.0 so.m^ w * JSCKS u6.8 *i5^a %$! " 

177 ^3*9 II ft*6 &I50*J |3.00 * 

ao ai7 68*45 * *|07 1146.4 ti.y? ** 

as 23^ 70*50 w uu.6 iHj).6 *.&A * 

33.6 365*1 73,61 ** ij7 iS77 *IS*M ^CUS I 
**73 3*7*os 76.03 *" $^f, a<t?ii fl,u * 

57.0 358*6 7l8 w 57t4 97.319 " 

66.7 40B*i|$ 8o3^ ** i69*a 9343.0 98.93 " 

74. S 4559 Sa.oa * 176. S M. pi, * 



Chretien tad Hoffer, 03S ^F of the 

found metastafele crystalllit of i/j wrt /s noi. of 

H f O at tenptr&tttrtf bet wets tit euttctic -|i,j **! * 6.8** 



loo fws. liquid 8ifttr Dioxide, S0 pl iliiwiltc 4.^7 At * 

tj lliipjwlu 1937,1 



725 



KALIUM 



SOLUBILITY OF POTASSIUM THIOCYANATE IN ACETONE, AMYL ALCOHOL, ETC. 

(von Laszcynski, 1894.) 

In Acetone. In Amyl Alcohol. In Ethyl Acetate. In Pyridine. 



Gms.KSCNper Gms. KSCN per Gms.KSCNper C 
t. 100 Gms. t. 100 Gms. t. 100 Gms. t. 


Jms.KSCN 
100 Gms. 


(CHaJaCO. 




CH U OH. 




CHaCOOCaHfi. 




CaHfiN. 


22 20-75 


13 


0.18 


O 


0.44 


O 


6-75 


58 2O.4O 


65 


1.34 


14 


0.40 


20 






IOO 


2.14 


79 


O.20 


58 


4-97 




133-5 


3-15 






97 


3-88 












115 


3.21 



EQUILIBRIUM IN THE SYSTRM POTASSIUM THIOCYANATB, 
TIRTIARY BUTYL ALCOHOL AND WATIR AT 25. 

(Olnnlnga. Herring and Webb, 1993.) 

The composition of the homogeneous mixture (plait point) of this system 
was found to be: 

37.9 percent KSCN 1- 19.3 percent ter. (CHIGOE + 42.8 percent H 2 

The original results for the remaining points on the binodal curve are 
not given but only the values of a series of arbitrary constants calcu- 
lated from them by means of empirical equations. 



SOLUBILITY OF POTASSIUM THIOCYANATE IN PYRIDINE. DETERMINED BY 
THE SYNTHETIC METHOD. 

(Wagner and Zerner, 1911.) 



t\ 

-42 
-42.1 
-42.4 

42.8 2.4 

43 .3 Eutec. 3.1 " +KSCN 
about +10 2.2 KSCN 



Gms. KSCN s Hd 

p Gms - pt * 

Mixture. rnasc. 


Gms. KSCN 
per loo Gms. 
Mixture. 


Solid 
Phase. 


O 


CAN 


70-71 
Il6~II7 
172.7 


I . 23 KSCN 
0.89 
at this temperature two Ii< 



layers appear and do not be- 
come homogeneous up to aoo". 



173.8 m. pt. loo 



KSCN 



loo gms. anhydrous acetonitrile dissolve 11.31 grns. KSCN at 18. 

(Naumann and Schier, 19x4.) 

Fusion-point data for mixtures of KSCN + NaSCN and KSCN 4- RbSCN 
are iven by Wrzesnewsky (19 1>). 



DISTRIBUTION OF POTASSIUM THIOCYANATE AT 17 BETWEEN WATER AND 
AMYL ALCOHOL. ( Wosnosucmsky, 1925.) 



MUlimols. KSCN per liter or 

ir a O layer (C t ). Alcohol layer (C,. 
1 55.4O 2.32t) 

338. 8a 7- <><><> 

410.753 



JlL.. 

88 
86 



Mlllhnols. KSCN per liter of 



layer (C t ). Alcohol layer (C 8 ). Cy*' 

64o.a35 17.379 86 

1075.2^,1 3i.5<)(> 86 



KALIUM 7Jft 

POTASSIUM CARBONATE K f OO g .l*H^Q 

SOMTBILITY or POTASSIUM CAIIOHATI in WATX*. 

(Mulder, 1864; <le Ooppet, i8?a; Mey*rhnffor, MCI<; K reman n -wcl 2itek, 
1909; fie tfaal, 1910; 0:*ikA 1910-1;}; B.tin, 1*137; Hill .1114 Hitler, J r%> ' 
1927; Hill, 1930* 1930UH. 



tef. K f 

IOC P* 



i pr 
* aol. 



-10 31.3 

-20 3* 

-30 3$9 

-36.5 39.6 
- 6.2 ir.pt. 50.9 

Si-as 

+10 51-0 

20 S3- 5 

25 2*85 

30 S3- 3 

The density of the 
350 r 1.560- Other . 

co ar " iven by """' 



Ice 



ill! 



**. 141, tut 

n t . ) 

*;n . H 

7.1 



W 



I jut 

I |il 

*:* - i nn 

I kit |*lfl 



wuh ihe 



ind At 



tifl 



w*i cvt- 

with the 
Mfl * 11 3 S * 



Ruhitxov, 1918, 

Appteby Ad Leishnan, 

deuee, based upon &n*ilysen of Hit #i **liil ph*itt*i lit 
liquid layers formed in the ^/^i * '^ H * * ! % 

that the stable hydrate in K.CO v aH^o ,%$ n*t K^^^ii 

Determinations of the ^pif ilirinn lit %|ii*<iti"i %iltiu 
carbonate and bicarbonate in Cfiictiuniii^frt j li* j*' ||', l. fit*r 
liter, in relation to the pAftUl prevmnf *f *(L tn Hi** ^AI pliAse in 
contact with the solution. Are gifn ty VUlker, *iy f ^<hnnion, 1927. 



POTASStUM 



KHCO, 



SOLUIIILITY OF POTAftSlUH !5!CA)lflOMAT1l IP 



(Dihiets, 18711; Rn^el, 4ii4 f^iih, j^ui. 4** Ptref4fttt, 

1909; Foerster, Bru^che mi Korberg-Sctttiix* i#j^, HtH ij Hilt, 1937; 

, 1929; Will, 19301*!; SiArkow*, 1*111 jwi l*tri*i 4ml 
1938.! 



The result* of tin* above tflve*Mg*tor* w*rif1 

from the swoottii > 4 ciirv^ from which the fi>IIiitig v.iln**** *rt* renl. 



tf. r 



100 



-0,70 





a. 17 


Ice 


Jtl 


1.17 4 


-3.16 





5-7? 


M 


3S 


I.lHH 


-3.31 


" 


9.98 


If 


10 


! , 1*1*1 


-3*90 





13. 6** 


IM 


lift 


1 p j}^ 


~S'<*3 


Eutec. 


16.95 


" * 










1.130 


18.6 




6d 





MO 


1.159 


Ji.8 


** 


70 






4 f '-!* t r Mia 

*f M|. ft* 1. OUFRMI 

jn,o KHOO, 



II ! 



727 KAIIUM K 



SOLUBILITY OP POTASSIUM CARBONATE AND OF POTASSIUM BICARBONATE 
EACH SEPARATELY IN WATER. 

<Ta*ahashi, 1927.) 
Results for Potassium Carbonate Results for Potassium Bicarbonate 

d. of 0s. K ? CO^ per Solid Q d. of Oms. KHCO^ per Solid 

1 sat. sol. 100 guns, sat. sol. Phase c sat. sol. 100 <5s. sat. sol. Phase 

"ii 1.533 50.45 K CO -2H o 1.1329 18.41 



- 5 



+ 5 

10 
30 
So 
70 



5445 50.93 10 1.1544 21.53 

546 51.35 " 20.51.1772 25.23 

5475 51.60 " 30 1.2004 28.52 

,549 51.90 " 40 1.2196 32.24 

.557 53.60 " 50 1.2439 36.04 

570 55.73 " 60 1.2711 39.65 

590 58.13 " 70 1.3005 43.37 



In the case of the Bicarbonate results the solutions were under a 
pressure of i atmosphere of C0 ? . 



Ci 



SOLUBILITY OF POTASSIUM CARBONATE AND OP BICARBONATE IN WATER IN CONTACT 
WITH ATMOSPHERES CONTAINING VARYING PERCENTAGES op CARBON DIOXIDE. 

(Taxahaahl, ig?7.) 

Results at 50 Results at 70 

Percent d, of OB*, per 100 Solid Percent d. of Qtos. per 100 Solid 

CO in *At. ga. aat. sol. Phase OOj, In s&t. w " 8 1^5tJ!f. 1 * Phft * e 

Acaospheres sol. / ^_A^-^~ V Atmospheres sol. ^0 CO^ 

o 1.570 38.00 17.78 KjpCjjaHjp o 1.590 39-65 18.48 K jpQf2HP 

16 1.569 37.90 18.07 " 22 1.588 39.34 19*41 "-RHC0 3 

18 1.570 37-43 17-90 M *KHCO S 26 1.575 39*02 19.16 " " 

20 1.512 35.81 17.27 KHC0 3 50 i-SSO 36.36 18.44 KH00 3 

22 1.494 31.79 15.80 " 55 1*430 29-47 16.85 

50 1.401 27.25 14.60 " 60 1.315 25.99 16.37 " 

60 1.352 23.32 14.20 " 80 1.335 22.65 16.18 " 

80 1.282 19.54 14.10 " 99.5 1-301 20.45 16.87 " 

99.5 1.241 16.95 14.62 " 



KALIUM 



7*8 



SoinBii.m OP PoTAaaiim CAim<AT* IN AQUIOU* SOI.KTIOKS or 

POTASSIOH BlCAIIIiONAT* AHB VlCt VilSA AT SVIAt TKHFtRATtlMS. 

H itvu 



Results at 5 



15 P 



CO 



1.543 


51 


53 


0- 





X. 


1 4 1 . 560 5 1 


5f 





*o 


Lli 


1.555 


50 


*S9 


1* 


7a 


H 


* 1.3. ill. $74 51 


Jill 


3 


a6 


" + 1,3, 




50 


.03 


1. 


77 


1 , 


3,ii 


*S*3 50 


-99 


3 


48 


1*2.11 


1.543 


49 


91 


1. 


90 


** 




564 50 


.5H 


3 


6a 


ti 


1.543 




*6$ 


u 


96 


M 


* 


ISli 511 


* 00 


3 


*93 


n 


1.509 


46 


*38 


a. 


$$ 


" 


* 556 49 


Si 


4 


.37 


H + Ml 


1.137 





.0 


30. 


15 


M 




S8 48 


*9'1 


4 


*37 


KHCO, 
















4i ;|7 


7! 


7 


*S^ 




Results At as 


339 33 


.04 


in 


.31 


M 
















.353 10 


.04 


33 


.10 


ft 


1.559 


53 


77 


0* 





K. 


li 


308 O 


.97 


38 


.83 





1.563 


51 


.33 


a* 


64 


w * 


i.a.il 


.300 a 


* il 


29 


.60 





1.562 


50 


.77 


a* 


85 


I. 


a.ii 










1-554 


50 


.38 


3- 


03 


w 




111 At 


$ 







1.549 


49 


,77 


3* 


23, 


*l 












1-545 


49 


.48 


3* 


33 





4 010), - S, 


*8 





.0 


k*,ii 


1.538 


48 


.14 


3,56 KNQO, 1.584 


1 


,8| 


11 * 3U3 


1.485 


42 


.8a 


if. 


67 


**' 


i*$Si $i 


97 


4 


.40 


1*21& 




34 


.71 


7. 


3S 





1.569 50 


93 


<i 


.97 


w 


1.316 


n 


-36 


13, 


If 


1* 


1.565 ^ 


.65 


s 


77 


w *!$0 


1.273 






15* 


4S 


t* 


-* o 


.0 


Si 


.3 


KHCO H 


1.228 


10 


.00 


19* 


3* 


If 












1.187 





.0 


26* 


7tt 


** 













Results for th^ ^ for ftii ft giv^n hy St*rlm,, 

1931, but the AWihor fallal 10 finl lit tiftttlil^ K^^.aXHCO^iiH^O. 

The earlier resului of itt|l *i 0* fftr ihi* *rt 

probably inaccurate his vAlut for K^CO y U WAii^r 4flts no |rtl; 

from that of ail otltr Iftii|*i0r:i 



OF t S 

CBLOUDI AHD or AT 30*. 



for 4- KQ, 

Gm. ptr io*> (ifu-i Sjf 



53.27 

52.22 
Si .'66 

1.64 

o 



ia 
o 

1,07 

96.32 
98.01 






KC1 



(Off 

|*rf to* 



3 8 SO 
2 OS 
O 





SI 77 
*<5 *4 

S5 7S 






f KOH. 

M^ 



KOH.IKP 



729 KALIUM K 

SOLUBILITY OF POTASSIUM CARBONATE IN AQUEOUS SOLUTIONS OF POTASSIUM 

CHLORATE AND VICE VERSA AT 24.i AND AT 40. ( Iljinsky, 1924. ) 
NOTE. Saturation was secured by active shaking at constant temperature. 
The attainment of equilibrium was controlled by successive density determinations 
and by analyses. In most cases the time required was 3 to 5 hours. For the 
triple points and those corresponding to double salts, several days were required. 
The solid phases were identified by analysis. 



Gms. per 1 00 gins. II 3 0. Gms. per lop gms. IL,0. 
sat. sol. KC10 3 . K S C0 3 . Solid Phase. sat. sol. KC10 3 . K 8 CO S . Solid Phase. 


Results at 24. 2. 


Results at 2-4. 2. 


r 


.55o 


o 


.0 


112 


.6 K,C0 3 .2H,O 


2. 


90 


23. 


4 KCIO, 




_ 


o 


.35 


in 


.6 +KC10 3 


.180 


3. 


00 


22. 


3 




_ 


o 


.5 


97 


.5 KC10 3 


. IOO 


4- 


5o 


IO. 


i 




- 


o 


.35 


96 


ft 


,o45 


8. 


IO 


O. 


o 


i 


. 5oo 


o 


.55 


95 


. 2 


Results 


at 40. 


i 


.362 


I 


. 10 


58 


.3 


.558 


o. 


o 


119. 


3 K*COi.2H 2 


i 


.362 


I 


.i5 


56 


.5 


.53 9 


2. 


2 


109. 


8 " +kcio s 


i 


.302 


I 


.60 


44 


7 w 


.3i6 


2 


I 


42.2 KC10 3 


i 


. 220 


2 


.20 


3i 


.3 


.195 


5. 


5 


24. 


4 


i 


.218 


2 


.40 


29 


.3 


.o 7 3 


14. 


2 


o. 


o 



EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, POTASSIUM CHLORATE, 
SODIUM CARBONATE, SODIUM CHLORATE AND WATER AT 24. 2. (Iljinski, 1024.) 

See note aboue 



Cms. per 100 gms. H a O 



cc 



a or 
sat. sol. 


K 8 CO a . 


K0l0 a . 


NA,CO a . 


NaClO a . 


_ 


0.0 


1.5 


22.0 


68. 9 


_ 


O.O 


2.6 


22 . 2 


66.9 


1.383 


o.o 


o.o 


24.6 


46.2 


- 


o.o 


>,.5 


24.5 


45.o 


1.398 


27.7 


0.7 


33.6 


o.o 


i.5i6 


89.9 


0.6 


7-7 


o.o 


i.5io 


90.7 


o.5 


6.7 


o.o 


i.53o 


9* -B 


0.4 


6.0 


o.o 


1.528 


100.7 


0.8 


1.3 


o.o 


1.552 


in. 6 


o.3 


o.o 


o.o 


_ 


o.o 


2.6 


22 . 2 


66.9 


1.442 


o.o 


5. i 


6.6 


88.2 


1.389 


o.o 


5.9 


3.8 


90.6 


1.443 


0.0 


5.i 


i.5 


95-7 


i.45o 


o.o 


4.6 


1.4 


96.0 


i. 32 


o.o 


4.2 


o.o 


96.6 


_ 


0.0 


2.5 


24.5 


45.0 


1.332 


0.0 


3.2 


26.0 


29. i 


- 


o.o 


7.2 


3o. 7 


o.o 


i.3 9 8 


27.7 


0.7 


33.6 


o.o 


1.433 


54.1 


0.6 


15.2 


o.o 


i.5i6 


89.9 


0.6 


7-7 


o.o 


- 


.0.0 


2.6 


22.2 


66.9 


- 


o.o 


a. 5 


24.5 


45.o 



Solid Phase 
NaClOg -+ Na s C0 3 .7H S 

-t-KClO, 

. 1 on a O~HNa 4 C0 8 . 711 S 
-hKClO, 



KClOj 



NnClO, 



NaCl0 8 



-Na a C0 3 .7H a O 



K KALIUM 



730 



CO 



EQUILIBRIUM in THI SYSTIH POTAHHHW 
POTASSIUM CH urn i0t AKD WAT sit 
mo MociotinfiQAvu, 19911.) 



Tn order to have an excess of GQ ? present, the Author* used for 
preparing the saturated solutions, water previously saturated'at about 

aPwith C0 ?l instead ol pure water. Saturation WAS thus affected uni 
i to 2 atmospheres pressure of C0 . " " r 



d. or 

UU 301. 



1.154 

1.175 

i 

i 

i 

i 



.195 
.181 



1.177 
1.184 
1.180 
1.198 
1.207 



Results at 

o.o 

9.08 

15.08 

23.93 

37.15 



37.78 

30.8? 

17.83 

13.75 

J3.55 

5.17 

0.0 



31.13 
Results at 20 



0.0 

10.05 

15*33 

34.31 



33* *9 
35*3*1 
&303 
19-35 
17*33 



KC1 



KCI 



KHOO, 



,3*8 



.197 



I. 317 
i.'i89 



31. u 
ii . 15 



o.o 

it . in 

17. 08 



(con. J 
i KMCO. 



10. od 
s.u 

0,0 



9. at KHCO. 



o.o KCI 



* 1$ 



5.5> KHCO, 
o.'g KCI 



\tl 



EQUILIBRIUM IN TUX S 

POTASSIUM CIILOIUDK, SODIUM 



K,a> a . 


""^"mnijjiM 

K.CI,. 


.\i",iaT 


,\* t u,. 


i 1^.57 


0..0 


O , II 


o^o' 


104.18 


o.o 


10,89 


f J . O 


3o-48 


o.o 


35.. $7 


f 1 , 


18.96 


0.0 


31,61 


o.o 


o.o 


o.o 


a * . 67 


*3/i 


0.0 


16.29 


o.o 


VW). 8H 


no.68 


a. 07 


0,0 


o.o 


o.o 


13.78 


7.45 


t5.Hi 


$5.79 


0,0 


*i7.o< 


10 % 


29.78 


o.o 


a7.(*fi 


8,^S 


ioa.5o 


1.83 


i i , era 


o.o 


36. 19 


o.o 


a7.Ha 


0,|| 


33.64 


<J7 


a5.7j> 


0,1* 


o.o 


aa.o8 


38.65 


o , o 



; : 4\t WAII-P At t^ t 
K|C :0| */i I 



m j.| 



j.7H,0 

'* 

ViHiO 



. Ki.l 



73i KAL1UM I 

100 gms. H2O dissolve 10.76 gms. K 2 CO 3 + 2.66 gms. KNO 3 at 10 when both 

salts are present in excess. (Kremann and Zitek, 1909.) 

100 gms. H 2 dissolve 10.53 gs. K 2 CO 3 +6.12 gms. Na 2 COa at 10 when 
both salts are present in excess (Kremann and Zitek, 1909). See also Potassium 
Sodium Carbonate. 

Data for aqueous solutions of K 2 CO 3 + KNO 3 + Na 2 CO 3 -f NaNOs, 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 K 2 CO 8 -f BaSCX <=* K 2 SO 4 + BaCO 3 at 25, 
80 and 100 are given by Meyerhoffer (1905). 

An aqueous solution, simultaneously saturated with K 2 COs.2H 2 O ? K 2 S(>4 and 
BaCO 3 , contains 53.1 gms. K 2 C0 8 -f 0.023 g^. K 2 SO 4 at 25. (Meyerhoffer, 1905.) 



EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE AMMONIA AND WATBR. 

(Applebey and Leishiaan. 1932.) 

Two liquid layers are formed at concentrations of ammonia above 2.5 
percent. The concentrations are expressed in gms. per 100 gms. sat, 
solution. 

Aqueous Layer Ammoniacal Layer Solid 

K^COg ' d.or sat. sol/NH^ KgCOg > Phase 



18.05 



25.06 



1 
1 
I 


-539 
517 
.507 




1 
1 


.0 

.06 

.57 


50. 
49. 
q8. 


69 
37 

84 







_ 






K 2 C0 3 . 2H? 


1 


.'1-83 


2 


51 


47. 


42 














H 


1 


475 


2 


52 


47. 


13 





.901 


32.07 


2. 


72 


II 


1 


./pi 


3 


.26 


42. 


54 





.921 


27.41 


2. 


99 




I 


371 


3 


.70 


39. 


4'{ 





.946 


24.59 


3 


73 




1 


340 


4 


.41 


35- 


95 





.968 


22.02 


5- 


84 




1 


.2/10 


6 


.91 


28. 


92 


1 


.038 


l6. 17 


12. 


44 




1 


. 1O9 


12 


.09 


18. 


51 


1 


. 109 


12.09 


18. 


51 


(critical solution) 









- 











42-9 


2. 


3 


K,CO,.aH,0 


1 


550 





.0 


51. 


72 







- 






M 


1 


-4S5 


2 


.88 


46. 


50 





.894 


30.48 


4- 


76 


M 


1 


M07 


2 


-75 


M3- 


6 





.917 


27 . 24 


5. 


98 




1 


404 


2 


.83 


42. 


78 





.919 


26.75 


6. 


15 




1 


353 


4 


.14 


39- 


31 





.950 


23.08 


8. 


87 




1 


. 104 


12 


.74 


21. 


05 


1 


.104 


12.74 


21. 


05 


(critical solution) 









- 











61.95 


2. 


10 


K ? CO s .aH ? 


1 


.556 





.0 


51- 


47 














f| 










-550 


50. 


91 














ti 







1 


.004 


50. 


91 














" 







1 


.286 


50. 


30 














" 







1 


.8^2 


49* 


77 














M 







2 


.885 


48. 


79 














II 







3 


-450 


47. 


00 







30.85 


4. 


83 


" 







4 


79 


40. 


69 







25.81 


7. 


48 









6 


.04 


36. 


36 







21.98 


10. 


85 









8 


.19 


30. 


94 







8.19 


30. 


94 


(critical solution) 



Experiments indicate that the upper critical solution temperature is 
probably above 155. It was also found that the vapor pressure of the 
two liquid layers in contact with K g C0 3 - 211^0 becomes greater than atmos- 
pheric at about 22.5. 



K KAL1UM 732 

SOUJUXLtTY OF POTASSIUM CAHHOHATI 

SOLUTIONS or POTASSIUM SULPATI AT 35 AHO VICE 

{Hill nd 



%, par 100 

pi*. ait, sol. 
" 



d.of 


QM pr 


wo 


oat. 


pis. mt 


ol. 


sol. 


/1 9 H T - *'~~ 1 


T; S ^ 


1.557 


0.0 


53.8 


1.557 


0.03 


S3. 8 


1.506 


0.03 


48.0 


1.465 


o.oB 


45-1 


1.348 


0.3 


35-0 



a. of 

Ml. 



1 . 230 

1 , 170 
t* 132 

I . I 03 

1.083 



1.5 
j.d 

4 . 9 
ft. 5 

10.7 



33. 



5*5 
0.0 



Solid 



POTASSIUM 



CO 



CAM01UTK 



SOLQIXLZTY Of POTASBXON HAONBSXUH 

AQ0I00S SOLtfTXONt Or ft)TASiIOM ClLOIXDl AT 
tM.) 



rJWOjwi*^ 



0.374 


0*0381 


0.790 


0.0353 


1*490 


0*0368 


a. 365 


0,0191 


3-38 


0.0139 



SOLUBILITY OF POTASMUM CAKMONATI: IN 
CAHBONATK AN VICIK VKIINA AT 
(!l|itkky, If It i 



XK 



Gin*, per 100 gnu, 
^^*U)0> !_ 


K^lioJ^ 


a%c:o s , Huttit 




Results at 11, 


84.4 
54.0 

38.1 
25-4 


o.o Kt<:n,.jttftO 

6.7 K,CO r NM* 

11.7 t-: 




Hesttlts at 4-iO" 


108.4 
io5.3 


o.o i s t;o, 

6! X,CO.!(ft 


So.o 


10.8 


35.4 


17.6 Nt,,0, 


o.o 


1 *i . O 




Results it *-4^ 


irjt.G 


o.o E,C:OI, 'iii,o 


no. i 


*A . 5 


1 08. 5 
107.4 
98.3 


9.5 

is! K,<:O,,N, 


9*. i 

48.4 
34. s 

28.3 


X <I O H 

18,7 

17.4 

33.i 



, 5 >S 


i HI 


i 


ii.ii 


.SS6 


IIH 


ti 


8.4 


- 


107 


r* 


$ i , i 


. 544 


Iflt 


t 


n. '1 


.1**7 


7 


II 


iti.1 


, *lii 




ll 


t f : * , -I 


.44* 


48 


'i 


M** , J 


, 4*ICl 


la 


I 


11.1 


! sif 


i** 


it) 


"1 i , ; 


'.lit 


i 


.8 


"ill , > 




ut 


it 


.{!. 


I , *! Sfl 


r : i 


. "i 


|1. t 


*,:; 


it* 


,i 


44- 



Hiiltif ! 

K,ro, N*I. 



,t:0|.H|0 



73 3 KALIUM 

Additional determinations upon this system are given by Kremano and 
Zitek, 1909, and by Osaka, 1910-11. These authors in common with 
Iljinski, 1924, report the formation of a hydrated double carbonate of 
potassium and sodium. The following later very careful determinations 
of Hill and Miller, Jr., 1927, show that at no temperature between 20 
and 50 is a hydrated double carbonate formed, but that the material 
which exists in contact with the saturated solutions is a hydrated 
soli4 solution, the composition of which can vary over a considerable 
range. Due to the. slowness with which equilibrium is reached, in all 
cases in which solid solution is formed, the authors found it necessary 
to prepare the mixtures in a special, manner which would reduce the 
length of time required for attainment of the internal equilibrium of 
the solid solution or anhydrous double compound. The saturated solu- 
tions were analyzed by evaporation to dryness and estimation of the H,,0 
by loss in weight. The total carbonates were determined by titration 
and from this result and the known weight of the mixed carbonates the 
percentage of each was calculated. The results are recorded in per- 
centage of H ? and Na^CO^. In the following table the K ? C0 3 values 

HpO * Na p SO from 100. 

Ons. per 100 gps. sat. sol. Solid 



have been obtained by subtracting the sum of 



d.of Ctos. per 100 gna. sat, sol. 
sat. sol. ' K.CO, Na_CO_ N 



Solid 
Phase 



d.of 
sat. sol. 



Results at 20 



Results at 25 (con. ) 






52 


.6 





.0 


K.ii" 


1.368 


10. 


1 


24.3* 


N.7 < 





49 


9 


3 


.0 


" + S 


1.369 


9. 


3 


24.3* 


" 




1.545 


49 


.0 


3 


.6 


S 


1.335 


4- 


4 


26.1* 


11 




1.541 


48 


.2 


3 


.6 


11 


1.317 


10. 


8 


22.9 


N.io 


1.417 


43 


.6 


7 


.6 


11 





6. 


1 


22.0 


it 




1.373 


17 


4 


19 


.0 


n 


1.263 


2. 


6 


22.4 


" 




1.375 


IS 


3 


21 


.1* 


li 





0. 





22.5 


11 




1.372 
1.371 


13 
17 


9 

.2 


22 
19 


.5* 

.2 


" + N.IO 


Results at 


30 






1.352 


16 


.0 


18 


.7 


N.io 





S3- 


2 


0.0 


K. 


i* 







.0 


17 


.8 


11 


.561 


50. 


2 


3.5 


" 




Results at 


25 






.561 
.554 


49. 
49. 


9 



4.0 
4.7 


M 

KN 


+ KN 


_ 


52 


.8 





.0 


K.iA 


.558 


48. 





5-4 


11 




1.561 


51 


.5 


2 


.8 


11 


553 


47. 


9 


5-3 


11 




1.555 


48 


4 


5 


.0 


" + S 


1.551 


46. 


2 


6.6 


" 




1-551 


47 


5 




9 


S 


1-547 


45- 


8 


6.8 


" 


+ N.i 


1.552 


'45 


.7 


S 


3 


It 


1-545 


45- 


i 


7.3 


N. 


i 




39 


4 


6 


.4 


It 


1.543 


44. 


85 


7.3 


N. 


i+S 


_ 


37 


. 1 


7 


. 2 


11 


530 


44. 


i 


7-3 


S 




1.471 


29 


5 


11 


.6 


11 


451 


33- 


4 


11.1 


n 




1.471 


26 


5 


13 


.6 


It 


.422 


23. 





18.5 


it 




i .406 


26 


.2 


13 


7 


" 


.419 


22. 


1 


19.1 


" 


+ N. i 


i . 404 


21 


.0 


17 


,9 


" 


.414 


21. 


2 


19.6 


N. 


i 


1-399 


16 


.4 


22 


. l 


II 


1.398 


16. 


2 


22.6 


n 




1.395 


15 


.8 


22 


.7 


" + N.7 


1.390 


13. 


5 


24-5 


n 






14 


.1 


23 


. 2 


N. 7 


1.378 


10. 


2 


26.6 


n 


+ N. 7 


1 .404 


12 


.6 


23 


3 


" 


1.354 


6. 


7 


27.8 


N. 


7 


1.368 


12 


.5 


23 


.3 


11 t N.io 


1.330 


4.0 


28.6 


it 


+ N.io 


o.o 


,28.0 


N. 


10 



K.ii = KpCO,.iiH ? 0; S = 
K P CO s :Na ? CO R varies from 
Na ? C0 3 .7H 2 0; N.i = Na 2 CO ? 



Solid Solution (Na 2 ,K 2 )C0 3 .6H 2 0, the mol. ratio 
1:0.88 to 1:2.07; N.io = Na 2 CO ? . loH^O; N-7 
.H 2 0; KN = K g C0 3 .Na 2 C0 3 . 



K KALIUM '- H 

SOUIflLITf Or POT A HS I I'M -- % A1I11MAT1 I* 

SODIUM CARHONATK AH Vir AT VAIH*' 

{Hill ift4 Htlivf. -'f. . *f 



ftf 



CO 



0.0 r fcs. Pr wo^*< 


, i* ui, -%4M d.r -to*. t-r i- |K. MI, ioi. ^ 


SIL, U r '^"^^" 


" ^/ 4 ' ? ,""" Wi *U **i* * *H^"S * ' ' M ^\*^ f 


ivmit^if . 


*" ''' - 4( ^ 


5^ 


I*.* 1 ^- '^ **"" , t.t il.ii K.] 


1.355 *7*S 


:!t KS i, *;<r /.! iilt) w 


45*1 


l,7 * N 4 I,N r J i|**,*> 4|.<| KN 


1 *f 1 1) 40 7 


/*. i X. i *** <if' , * 7 * 


i.fi^tl )Bo 


4 * . * * / I * 'i " * J " 


1 479 17 * i> 


lu.ti * * i .<HM * )Ji M. 


14S4 V?S 


II,* ' .i'i* i^ 1 ! u<| " 


*4SS 14* a 


1^,0 * . ut jt i*i H, a * 


1*454 I*!* 1 ! 


I J , tl " * S . i . 19 .' Ji I * 1 " 


1.457 *0.<> 


ui.ii v .i - .* ii, a w 


1 . 1446 J? - H 


!*. f * " /r*aM-* .1 Ml 11 


1.377 M.H 

1.354 4.7 


*.* '* . ,, 

..,., " * v - ' - k ; 

II S.v 1 *? f * 1 1. I 


""" 0O 


! . * tt pi , * H,u KN 




i . M 'U. r - Hs N, 




.< u.j w 


K.xi = K CO,.i*H, 


f); t; - :Uilil ^Ui>' f%i, t K,i 'u-rM^*. lit** wL 


rat ia K f Cn s :fU f t*o', 


Afit**4 ftMf, tin,'*.* !'* ',**?. **. t ' K.4^D1,it)| 


N.7 NApCO^Hp'); 


,*4i * XV'O.T^K ^ %i ; K, ^I^.'M* *'*. 



for 



or 



Great WAS rrc,t'4*! HI <*** tiring 

alum 4d mSiii W4^ d*tir?urtt r*y *rt|*f> 

dettPiiRtil A 
Rd its 



i*. ! ^?** ciwiiiatil p 
J i i ir>, Ti* 



f ,.* 



4. or C 

WU Ml* ^ 


*T3*>?**wC 1 '* -' "'-"I-.. ' 


*";"/" r ',^^ 


* 


5 'i * 9 u w K * 1 1 i.ii* 


,, .. n.H N 


i . 583 


51 .*! j? '" i * 1 4"* 


i t , i jm . r l 


i. $81 


50.7 l.ri '" *^ >. N 


I | jC,ii* N 


1.586 


48. 1 ,.i ^ t , r ,*. 


81 , *s jHs* 


i . 563 


4^* I 1 f* rf ** | . Ml * 


* rf J J } f'l V1 


1.562 


4*1*4 7* * ** * ^ S i . m S 


'. i !*?. 


K550 


4Ji8 *l* J ^ S 1 J'l ^ 


* , ^ I , f i 


1.508 


37*1 0.*, ** >.//t 


< r JJ1 


1.496 


Jl.l t|.^ " .*." ^ 


t , JJ.1 


1.4S* 


37*1 !,*, " .,"^ 


l, 4 ^ ^*.H 


1*42^ 


3i| 1 l67 " i . *rf^ 


J, ! |sj 




t * i^ 1 


t, 4 it a 



co 



735 



POTASSIUM CARBONATE 



KALIUM 



Data for eq.uil.ibri urn in the system, 

K ? C0 3 + 2NaHG0 3 - 2KHC0 3 + Na ? CQ 3 in water at 25 , are 
given by Hill and Smith, 1929. 

The authors first give the previously determined data for the four 3 
component systems; K-COj, + Na-COj, * H 0, K ? CO^ + KHCO, + H ? 0, KHCO, * 
NaHCO^ + H.,0 and Na p CO^ + NaHCO,/ H ? 0, calculated to' gram mols. per 
1000 gm. mols. H ? 0. They then report their results for saturated solu- 
tions each composed of water and three of the above four compounds-arid 
in contact with two or three of the several solid phases which exist at 
25. The results show the location of in curves representing the solu- 
bility equilibrium existing with two solid phases, and of seven iso- 
thermal invariant points at which the solution is in equilibrium with 3 
solid phases. A new tetragene salt was found, having the formula K ? C0 3 - 
NaHC0 3 .2H ? and not occurring in any of the 3 component systems. 

In a later paper Hill, 1930 gives results for double salt formation 
among the carbonates and bicarbonates of potassium and sodium at 25 
and at 35. The partial isotherms show that the double salt K ? CO . 
2KHC0 3 .i4!l ? ami the tetragone salt K ? C0 3 .NaHC0 3 . 2H ? both exist, at 
these* two temperatures. 



POTASSIUM Ri CARBON&Tf? 

SOLUBILITY OF POTASSIUM BICARBONATE IN AQTTROUS 
SOLUTIONS op SODIITM BICARBONATE AND VICE VEPSA. 

(Oglesby, 19P9.) 

Carbon dioxide was bubbled through the solutions prior to the period 
of saturation and afterwards an atmosphere of C0 ? was maintained above 
the surface of the solutions. The analyses were made by titrating the 
total alkali with HC1 and determining the K by the perchloric acid method. 



d, of 


Qraa. per 100 


gjns. sat. 


sac. sol. 


r N4HCO, 


KHCO, ( 




Results at 


20 


1.1777 


0.00 


24.98 


1. 1830 


1.38 


24.32 


1.1897 


2.84 


23.58 


1.1966 


4-37 


22.89 


1.1803 


4.58 


20.48 


1.1637 


4.88 


17.98 


1.1519 


5.16 


l6. 1$ 


1.1309 


5-73 


12.72 


1*095*1 


7.05 


6.45 


1.0625 


8.72 


0.00 




Results at 


25 


1.1882 


0.00 


26.78 


1.1927 


1.12 


26 . 1 3 


1.1977 


2.39 


25.56 


1. 1998 


2.72 


25.27 


1 .2042 


3.74 


24.93 


1.2087 


4.63 


24.46 



d.of fltas. per loo aus. suu sol. Solid 
sai. sol. ^NaHCQ- KHCO """"""* Phase 



Resul ts at 25 (Con. ) 



KHOO 



1.1903 4.94 



"+NaHCO, 
NaHOL 



i. 1732 
1.1547 
i. 1282 
1.1035 

1.0648 



5-14 
S.62 
6.38 
7.41 
8.20 

9.34 



KUCO 





1.1988 


0.0 




1.2077 


2.06 




1.2145 


3.58 


( 3 


1.2189 


4.83 




1.1887 


5.47 




1. 1543 


6.23 




1. 1196 


7-34 




1.0973 


8.22 


NaHCO, 

o 


1 .0673 


9.95 



21.89 NaHOO^ 



19-39 
16.46 

12. 10 

7.63 
4-23 
0,00 



Resul ts at 30 



28.52 

27 . 43 

26.66 

26.01 

21 . 40 

16.08 

10.22 

6.18 

0.0 



"fNaHCO- 
NaHCTL * 



K KALIUM 



736 



EQUILIBRIUM IN THE SYSTEM POTASSIUM CAKIIONATI^ SODIUM CARBONATE, 
POTASSIUM SULFATK, Sooir SI'LFATE ANI> WATER AT iti, 

s HliHtiiU\ ttW i 



Cms. 



P S&O 



. n,0. 



K $ C0 3 . 


NMI0*. 


" i 9 so,, Ht f 


o. 


O.O 


17.44 


o . o % \ 


.<>6 


o.o 

0.0 


O.O 

o.o 


;!: ; ti :< ( 


.Hf> 


3.58 

7 .3 7 
18. 5o 


26, 09 

33,74 

35.63 


O.O ^ f 

B.'io < 


:;: <! 


27.07 


35,35 
io,83 


o.o I 
1.36 < 


.<! 
1.0 


35 '.7 1 
o.o 


1*7. 38 


0.97 < 
<)..$o 3 


1.0 

.31 



> gms. Aq. H6.5*/ Olyccrol (</ 
f)8.5/ w (' 



Sll<l !*, 



K.Stl, 

.\;to, 



NiiSo,,njir s o 



dintolve ^o.S gm*. K 3 (*.O A at w*. 

ifi*4 M ^ 

f Hotm. WMM3.) 



CO 



EQUILIBRIUM IN THE SYSTEM POTASHIOM CAXKOKATE, METHYL ALCOHOL, 
WATER AT a3**-a<>. 

(Fnnkfofttr ftad Fiy 191.1-) 

The authors give the for the binudiit curve the quadruple points 

but tie lines, other than for the quadruple point*, not dnermtned. 



Cms, per ux> Gmt, Hofm9mous Lk|ttifi 



% 


7S-SS 


IT^' 


6.91 


63.13 


29-97 


8.07 


50-26 


32,67 


10.17 


52,64 


35-33 


12.03 


40-97 


37- QQ 


14,24 


45-74 


40,0,' 


16,48 


41.76 


41.76 


18.89 


37.76 


43' 36 



Upper ejtuwL point. 



at .61 

23. IS 

30,73 

40.65 
4J Q* 

411,05 
f tower *|tttt 



(*!., tr tec (im*. f!nmtitrnrmi* Liipid, 



44.^6 
45-60 

47-04 
4-7i 

40, 80 
50-00 

40-09 
47-% 
44,81! 



3.1 4 ,\ 
3 1 . 26 

to 57 

17 ^7 
ci.Jd 

6 U 

d t 



Tlie following results for the tolubility of KtC"C> in <*0ncentrntiont 0! aq. 

CHtOH above and below those yielding liquid kyew arc* giv 

Cms. per 100 Grot. Sat. So). <m* fwr ifl*^ <* Stt. Sot 



^03 51,30 

2 -22 50- 33 

6,1 40. 05 

Two Liquid Laywa Formed Here. 

7S*8s 6.32 



s 

80 



i 56 

1 e>S 

2 72 
S 7 



737 KALIUM 

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. 

Cms per 100 Cms. Upper Layer. Cms per 100 Cms. Lower Layer. 



K 2 C0 3 . CHsOH. H 2 O. K 2 CO a . CH 3 OH. H.,O. 

30 21.7 42.2 36.1 

20 13.8 52.1 34.1 

20 12.4 ... .... 44.2 8.2 47-6 

o 7.6 66.3 26.1 46.3 6.7 47 

o 7.4 ... ... 46. 6 6.6 46. 8 

+ 17 6.2 69.6 24.2 48.3 5.7 46" 

35 $ 72.9 22.1 51 4.3 44.7 

EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, POTASSIUM DIPROPYL 
MALONATE AND WATER AT 25. 

(M 'David, 1909-10.) 

A series of mixtures of K 2 CO 3 + KCnHwOi + H 2 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. 

Gms. per too Cms. Upper Layer. Cms. per 100 Cms. Lower Layer. 

K 2 C0 3 . KC U H 19 4 . H 2 O. K 3 CO a . K.CnH 1B Q<. HA 

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 0.5 64-5 

7-2 50-5 42.3 33-5 o-9 <>5.6 

8.7 39.2 52.1 28.9 0.7 70.4 

ii 34-6 54.4 26.8 0.8 72.4 

14-5 23.5 62 24.8 3 72.2 

17 18.6 64.4 23.1 6.05 70.85 

18.6 15 66.4 21.7 8.7 69.6 

Several determinations at 2 and at 56 are also given. 
EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ETHYL ALCOHOL AND 

WATER AT 23-26. (Frankforter and Frary, 1913.) 

NOTE. The binodal curve for the system was very 

carefully determined and tie lines were located by estimations of KiCOs in spe- 



cially prepared conjugated liquids. The original results have been plotted and 
the following data for the conjugated layers read from the curve; 

Alcohol Rich Layer (Upper) Water Rich Layer (Lower.) 
Cms. per 100 Gms. Solution. Gms. per too Gms. Solution. 

,_,, A- - -, .,..,. - * ----- - - 


KCO a . C a HOH. H 2 O. 
0.095 90-65 9-2S5t 
0.241 72.7 27.059 
i-72 53-5 44.78 
4.03 42.6 53.37 
6-30 35-5 58.2 
8.29 31 60.71 
10.35 2*7 62.65 
14.2 20.5 65.3 


536" 
39-H 
29.62 

25-7 
21.08 

19.15 
18.18 

14.2 


o". 28 
i 
4 
6.4 
ii 
13-2 

14.7 
20.5 


H,0, 
4<J.I21 
50. 8g 
66.38 
67.9 
67.92 
67.65 

67. 12 
65.3* 





* Plait point. t Quad, point. 

The authors give a complete summary of previous investigations of this system 
by de Bruyn (1899, 1900); Bell (1905); Cuno (1908-09). 



K KALI UN ^ g 

Data for the ronjiiKaU'd H|"l layi'r* obtained in the system potassium car- 
bonate, ethyl alcohol and water at 17 and at ,*5" an* i:svni hv de Brttvrt (1900) 
and at '20, 40 and 60 by <'uno injoX). 

COMPOSITION OF THE CoNjt'i.AiLi) LKK-JUS \vinru A HI-. i\ KvnuuuirM WITH 
SOLID POTASSIUM CARBONATI-: iyi f ,uRiTi,i', POINIV .u Y^ioi/Hl>,Mf'KK,\ HIKES. 

uU* ilt'uvn, I<MJ i 
Cms. IX.T too Urns. UHXT Luc* 



-18 


0.03 


cp J 


t) 7 


o 


0,04 


ul .t) 


K.I 


+ 17 


0,06 


gi-5 


H 4 


35 


0.07 


tp.C) 


<) 


50 


0.09 


gi.8 


K ! 


75 


o. u 


91,4 


S.5 



II4I. K t M t Mt.UH il/l. 

O ,' 48,6 

O J 4 H.$ 

o ,' 47.7 

o ,* 46.4 

o ,i 44.5 

o *' 4 i.g 

, SYVTI'.M PoTA-^ITM t *AHIU>\'.\ I T., A* I-'IONI-., W.AU'iR AT JO n . 

The binoclal euive was verv eaiehillv determiui-d and, in .idditinn, data fni the 
quadruple points Isoltil IvjOU ani tivf fir line'* \\-tr l*H-.tird Tlu--.r data wen 1 
plotted and tin* iollowhu; iuterpolateit valuv* IMI tin- t itujti^.tted litjutds read 
from the curve. 



(CIl i'}/'CK H,< K,'(, tf!I,<,n. ||,o 

0,0024 <)<>' 4 .* ?J H ^** ? lr>|ir 4V (i l 

0.030 4 .** li(l -^ fl -* f *' flf> '? 

0,712 55 ,* 4J *)) -4 4 ,f V Vi l 

1,36 48 S f M - ? - *> 4 V V - .*0 

4,57 34 ft i 43 f * )^ s ?>? -' V/ HH 

6,97 27,5 CIK ;n 14 yy 1,4 yj ,,| 

10,5 20 ftr.s* *'' * ^ o*)'S 

* I'kit (Mttttl. f yiMit i4t$l. 



Additional nsullH for the bimetal .-urv.* .it ^i aj - K% % ? rrntH! :*dli t i- 
factorily with the *bovt, are uivt*n !>^ If-i-^ufHS i*u*; i7 t, flu * ailur 
mentions that lht effect of fitff*fMf urr *ij* ui* r':mli* i* .-ilttiiii, 

EQUILIUKIUM IN TK SwrEM I^IA-^H'M I'AKHONAII-., NUKMAI. PHOI-VU 

Au:t)tlol, ANt WAttiK AT dt" ^r'\ 



The auth 


ors give the 


data for iltt* bintwliii fuivi' ,i 


but tic lines wen* not ItH'att'd. 


CJms. IKT 


tootitm. llw>: 


flHMiut WlfUPl. . 1 |' 1 * 


^7 % " """"* 


-..a,,,,,,...,...,,:-.., ,. ......A. 


" 'i 




c*iiI}C)Il, 


t! |O, i* < < * 


52,0 


0,0,1 


47- o* i i* 


46 . g8 


O. IJt 


5J .gi *> J ii 


30 


O .'O 


(K> *%* 4 / i 


34,58 


O . !O 


{15, 15 \ ^t 


30 43 


0-4$ 


CM) I J ^ I I 


30. "J I 


0,78 


7,? 71 $< 


22, Hr 


1.32 


75 87 I M 


IQ.OS 


a.^t 


78 (U I t i 


10,35 


3 . ^4 


to 41 i i| 


13.47 


4 41 


K,?. IJ o iifH 


10. QO 


6,24 


Hi 77 o i<y 



,15 41 
4 



739 KALIUM 

EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ISOPROPYL ALCOHOL 

AND WATER AT 20. 

(Frankforter and Temple, 1915.) 

NOTE. The results for the binodal curve in this and the following system are 
reported in terms of gms. per 100 gms. solvent (water + alcohol) instead of gms. 
per 100 gms. of homogeneous liquid (K^COa + water + alcohol.) 

Gms. per 100 Gins. Alcohol + Water. Gms. per too Gms. Alcohol -f Water. 

K 2 C0 3 . Alcohol. Water. K 8 CO a . Alcohol. Water. 

44.844 2.911 97-089 15.021 IQ-445 ^0-555 

36.137 4,783 95-217 13-244 23.910 76.081 

28.879 7-349 92.651 6.065 45-397 54-6O3 

24-152 9-*59 90-841 3-033 53-265 46.735 

17.665 14-395 85.605 2.954 57-294 42.706 



EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE 
Iso PROPYL ALCOHOL AND WATER AT 25 

(Ginnlngs and Qieta, 1931.) 

The binodal curve, a tie line and the plait point were carefully 
determined. 

Ctas. per too sns. of Uie three constituents Qas. per 100 ns. of the direa constituents 

"' x ~ ~~~"~" "" 



o.io 69.60* 13.86 10.10 

2.80 42.20 19.83 4.42 

6.04 28.40 25.50 1.93 

6.2 27.8 PP 33-20 0.65 

9.65 17.25 52.67 0-23* 

* Tie line which shows the composition of each of two liquid layers 
in contact with each other. The one being the upper, rich in iso 
propyl alcohol and the other, the lower, rich in K p CO s . 

PP is the plait point which shows the composition at that point, on 
the binodal curve where the two layers merge into a homogeneous liquid. 

EQUILIBRIUM IN THE SYSTEM POTASSIUM CARBONATE, ALLYL ALCOHOL AND 

WATER AT 20. 

(Frankfurter ami Temple, 191:5.) 
Gms. per roo Gms. Alcohol -H Water. Gms. per 100 Gms. Alcohol + Water. 

K 2 C0 3 . Alcohol. Water. K s ('O a . Alcohol . Water? 

47.746 2.103 97-#97 8 ."239 30.677 60.323 

33.200 5.267 94-733 5 -S3 r 39-337 60,663 

23.486 9-309 00.691 2.020 54.487 45 513 

16.354 15-037 84.063 1.015 62.610 37-390 

11.331 22.454 77-546 0.0853 81.228 18.772 



The binodal curve for this system at 25 has also been determine'! 
by Ginning?; and Dees, 1935, but the authors do not give their experi- 
mental results but only a series of arbitrary constants calculated 
from them by means of an empirical equation. From these the conclu- 
sion is drawn that ally! alcohol seems to be more difficult to salt 
out than either iso propyl or normal propyl alcohol. 



K KALIUM 740 

POTASSIUM 0AR80IUTE 

EQUILIBRIUM iw TIE STSTIH PmrAsaxtm CARBON ATI, TIRTURY 
BUTYL ALCOHOL AVD WATER AT 30. 
rtti 



The points on the hi nodal curve were determined by observing the ap- 
pearance or disappearance of clouding in a mixture of wei glued amounts 
of salt and one of the liquids, upon Addition of * weighed amount of the 
other. The conjugated points were found by preparing mixtures which 
yielded two liquid layers and Analyzing for sail content. The 

plait point, P*P. , was found by plotting* The following results are 
those given in the authors 1 table under the column heading K f S0 4 which 
was evidently intended for ^ f CB 3 * 







in butft&ol rich I* uli rieto phaat 

69 34*2 

li a an. . n 

a? i.aPP. 



In a later paper by Glnoings, Herring aat Vebb, 1933* l ^* values given 
for the plait point, P*P* we rtspec lively., 

2,3 percent K f Q) 3 and 36,3 percent fCllgJ^COff inteail of 3.3 and 2.7 
as shown above, 

The binodal curve and plait point of the *yftt*m 

K^OOjj Pyridine * H t O At 35 
has been determined by Ginnlnfs, and tfinohAra., 1933. but the 

authors do not give their experimental rtsultst t>ui only" the vAlnes of 
a series of constants calcolated fro* then by of tup! Heal 

equations. 
Data for equilibrium in the of 

KLOO. * Pb0 * KCrO * f^c:r0 t IIO at 3* 
are given by Goldblnw and toifllA 



loo cc. anhydrous hydraxine i gm. K^Cik at room temp, 

tnn 



(WtliHtnn Rwttoamt, 1915.) 



... , (tiHtnn Rwttoamt, 1915.) 

ioo gma. aqueous solution annulttneouily Mt. with Ki(:Oi mncl cane at 

1^5 contain 23.24 gms. KCCX and 36 gm& sugar. ' dCoUtr. 18974 

Fi^ng-mnt data for mixtures of KfCQi + KCUmI K,CC>i + Nad (Sackur, 
l l\*~ l rk n*r& + n KiSC l l (Anmdorl, 1913; U Chatdier, 1894); KtCO, 

i (Le Chateiier, 1894). It* chticttcr, 1814.) 



POTASSIUM TOAHYL OJ^BOHATl 

ioo gms. HsO dissolve 74 gms. salt at 15*. 



74i KALIUM K 

POTASSIUM OXALATE K 2 C 2 4 .H 2 0. 

FREEZING-POINTS OF AQUEOUS SOLUTIONS OF POTASSIUM OXALATE. 
(Klein and Svanberg, 1920.) 

t" O.Uli. 1.000. 2.08S. 

Gms. KoC^Oi per 100 cc. solution . 1.271 4.177 8.355 

SOLUBILITY OF POTASSIUM OXALATE IN WATER. ( Woskrcsscnskaja, 1926.) 

Saturation was secured by constant stirring for 2 to 4 hours, and repeating the 
determinations after stirring another I 1 / 2 hours. Below o the determinations 
were made by the freezing-point method. 

Gms. K S C 2 4 Cms. K a C s O,i 

per 100 gms. por joo gms. 

t. sat. sol. Solid Phase. t". sat. sol. Solid Phase. 

o.o o.o Ice 20 25-95(23.80) K 2 G 2 0.i..H20 

0.6 2.4 25 27 . 4o 

1.4 5.i4 3o .28.70 

3.o 10.47 J) 4o 3 1. 2 

4.0 14.10 5o 33.5 

5.o5 17:12 60 35.6 

5.70 i8.83 70 37.8 

6.34 K, lire. 2O.OO fr-t-KiCjOi.HaO 80 4O.2 

o 20.28 K^CgOt.IIjO 90 42.0 > 

10 23.20 too 44.5 > 

16 24.81 107 45.9 

The result in parenthesis is given by Trifonov, 1924, 1925. 

SOLUBILITY OF MIXTURES OF POTASSIUM OXALATE AND OXALIC ACID IN CO 

WATER AT 25. 

(Foote and Andrew, 1905.) 
Gms. per TOO Cms. Solution. Mote, per too Mols. HA <, ... _, 



IO.2 ... 2.274 

10.31 O.O4 2.302 0.005 H 2 CA.2H 2 Q4-H 3 K(CA)2.2H S O 

9.26 0.13 2.046 O.Ol6 

3.39 0.63 0.707 0.071 

2.06 4.26 0.440 0.495 H 3 K(CA).2H 2 0+HKCA 

1 . 10 1 1 . 50 . 200 1.427 1 Double sak HKCa Q 4 

0.99 16.93 0.240 2.235 J 

0.85 21. 08 0.221 2.928 HKC 2 O 4 +H a IC4(CA)i.2HiO 

O.82 21.49 O.2II 2.998 | 

0.64 2 3'52 O.I 69 3*36l f Double salt HaK^CA^.aHaO 

0.57 24.88 0.153 3-6I7 I 

0.43 27.52 0.122 4.14 HR 4 (C04)i>H0+K>C|0'H/> 

27.40 ... 4.09 K,CAHjO 

SOLUBILITY OF POTASSIUM TETROXALATE, KHsCCaO^^HaO, IN WATER. 

(Koppel and Cahn, 1908.) 
*" ^S^O 8 . ^ S<> Hd Phaa ^- 

0.25 cryohydrate o . 99 KHt(CA)a. aHjO 

o 1.27 " 

30 4.30 

60 11.95 

iQ3.5b.pt. 72.17 

100 gms. methyl alcohol dissolve 2.07 gms. KH (C.Oj, at 15 and 
1.55 gms. at the b. pt. f 66.4. 

100 gms. acetone dissolve 2.^4 gms. KH(C p 4 )^ at 15. (Henstock, 1934.) 



K KALIUM 



742 

IN TUB MM' KM PoTASSIfM <>X \LAtK, O.XAUC Atl!, WATER AT 

O w , ^O" AND I to'. 



COO 



Results at o. 

Gms. JX.T mo Gnis. 
Sat. Sol. 


(Kttppel Aa4 Calm, t'.ia.i 
Results at 30. Results; 

(into. i KM' lort CiiiiH, t*!ii.. JKT i 
S,it, S.I >.it 


,U 60". 

S " J So!i.| PIUMMU I'^t-h Case. 


CA- 

2.72 


" k a o. ' c A. 

07 


kail. fa* 
2.|. 


75 


K f!' H,CVWIM 


2.QI 


0.226* 


IO. 


1-5 


O. IO 




i 


2 '.827 


o, 125 


IO. 


2J 


c,,i4 25 


70 


ci 46 *' ! KII/f,0 4 >.3Hjt> 


2 345 


0,145 












1.471 


0.105 


7- 


28 


o 3s 


So 


ti t | KH.'t iO.ij.all^O 


0.823 


0.240 


4 




ft 


tr> 


t> V S 


0.799 


0.454 


.* 


08 


O t sO -'> 


S 7 


o <r; 


1.173 


0.785 


2 


48 


t OO. 1 | 


1 ; 


onu 


1.381 


0.062 


2 


i)H 


i . 70 o 


S ' 


i |S 


i. 545 


i . 155 






Cs 


i ; 


.' .-4-1 


1.666 


i . 273 


4. 


24 


2.76 o 


r/ 


S 60 " * KHi'A 


1.754 


1.470 


4. 


26 


3 . ^8 H . 


Hi 


C> 37 k!!i"4! 4 


2.627 


2.858 


S- 


44 


5 4i 10. 


17 


to 


3.772 


4.422 


6. 


6ft 


7 ; s ,' 


3(> 


13 40 


4,202 


S. 161 


8.64 


10 o^ 4 


10 


!fl 


4-075 


6,088 


10, 


.03 


I ! O i M 


t ; 


,7 So " 


5.652 


7 


10 


,Ho 


j. 04 U> 


07 


I.S S> s ! K : t *,'. 114. j0 4 ,j!i)( 


6.27 


7.87 


II 


-47 


14. s i 10 


it 


ii ;tj iK- AI ; it.i ti 4 jll/t 


7-63 


0,72 


I.! 


i<> 


15,11 ici 


.80 


JO, iij 


8.66 


it, 14 


12 


.$* 


X$ 37 i(* 


)> 


.o ,u 


0.055 


11.58 


12 


,1)0 


16. ^3 17 


I,| 


'O 7-i " f K ;*'*>, |f.ii 


8.826 


11.52 


U 


.,0 


1 6 14 ifi 


'/I 


jo,4i K.-i/iJI/l 


5,215 


"33 


8 


52 


i 5 . 03 i 5 


.<M 


2O 1 1 


2.23 


14.80 


4 


, <;$ 


15-55 *S 


Of) 


HI 66 


1.245 


16.82 


I 


.87 


18.17 8 


S,! 


ig ri 


0.871 


18.4 





.74 


22,32 


. 04 


J.J.Ot) 


0.511 


2O.Q1 


, 




o 


. 4 14 


2t) 


0-325 


23.30 






o 


305 


3 f . 40 


o 


4** 3t 


o 


46.79 o 




51.34 KOH 1!;CI 


* SupcnuLturatcd. 


f Attmtf. 


EQUILIBRIUM IN 


THE 


SYHTH 


.M POTAHMt'M Ox\!.M'l\, OxAI.H* At H t \\'All\K 










AT 25* 


' 




(Hartley, I>n 


utKmtn, Vlitkntl anl Bttrili!iuit I',IM-) 


Cms. per itoo Oms, 


(*mi pr 


inn (\ 


ttt% 


Stt Sol. 


Solid Phut. 






^tlit I'lii-.f, 


CA- 


K a O. 






*"< jCi 


* j- 


77* 


8.2Q 


Hf 


41)4. j I) 


faO 


^.O- 1 *) 


J 


o".* KH}ttV>i>j jHit) 


8.278 


0.045 "' 


fKII s i 


cr s o 4 ) a ,j 


Hjt> 3-4f|0 


-?. 


360 Qt | KfUV^i 


7.412 


0.064 


KHa(( 


VWs.^Ii 


laO 3 7H 


H 


too KIIiV 4 


2.827 


0.238 






5-457 


S 


t)!>) 


2.OO7 


0.346 




a 


g.8i6 


I f 


*K> " i jKjCVj H,(.V\ "H.-O 


1-734 


0.567 




< 


1^.465 


i ^ 


7 t a K,i '/ , 1 {,< %t i t j 1 !, i * k ? " .0, 1 1 


2.675 


1.714 




41 


II, 85 


15 


i! K,cv>, !!,ii 



Similar data at 15 for the above system arc given by |tifinfltn-'h ,itni I.a 



743 KAUOM 

SOLUBILITIES IN THE SYSTEM POTASSIUM OXALATE, OXALIC ACID, WATER AT 
THE CRYOHYDRIC POINTS. 

(Koppel and Cahn, 1908,) 
(Temp, of Equilibrium of Solution with Ice.) 



K 



toIce 
Separa- 
tion. 

-0.95 
0.90 
-0.52 
-0.25 
0.58 
-0.78 
-1.50 
2.IO 
-2. 7 8 

-3-45 


Gms. per ioo 
Gms. Sat. Sol. 


Solid Phase, 
Ice 4: 

H 2 CjO4 . 2 MjO 

4 K. HS ( CjO<) j 
K US ( C-jO^) j . 2 rI 8 O 

" 4KHCA 
KHCA 


CA. -KaO. 

2.720 0.0466 
1.672 0.0602 
0.643 0.210 
1.229 0.823 
1.648 1.234 
2.707 2.950 
3.687 4.363 
4.576 5.50 
5.68l 7,05 



f of Ice 
Separa- 
tion. 

~ 4-45 
- 5.20 

- 5-32 
- 5-97 
- 6.55 
8.10 
10.30 
13.60 
17.40 
-23.80 


Gms. 
Gms. 


per ioo 
Sat. Sol. 


Solid Phase, 
Ice4: 

K 2 CA)*H 8 CA.2l 

" 4K.CA.BW) 
K 2 CA.H S 

M 


6.902 
7.616 
7.696 
8. 5 I 
6.742 

4.999 
3.358 
1.854 
1,200 
0.606 


KA ' 
8.820 ( 
9-74 
9.84 
1 1. or 
10.45 
10.86 
11.76 
13.08 

14.55 
16.89 



SOLUBILITIES IN THE SYSTEM POTASSIUM OXALATE, OXALIC ACID, WATER AT 

THE BOILING POINTS. 

(Koppel and Cahn, 1908.) 



tof 
B. pt. 

105.5 
104.9 

104.3 
103.4 
102.9 
102.5 
102.4 



Gms. per ioo Gms. 

Sat. Sol. 



Solid Phase. 



' CA- 
39.84 
36.95 
3 2 .75 
27.64 
27.46 
23.36 
18.81 



KA 
5-25 
5.83 
5-97 
9.12 

H-43 
10.50 
12.29 



"+KHCA 
KHCA 



t'of 
B.pt. 


Gms. per ioo Gms. 
Sat. Sol. 


CA. 


K 2 0. 


102.8 


19.10 


18.25 


103.25 


21. II 


21.71 


107.7 


25.19 


27,9* 


106.35 


22.04 


26.45 


106.25 


19.17 


25.02 


108.25 


12.73 


27.69 


m.8 


5-35 


30.40 



Solid Phase. 
KHCA 



cc 



From the preceding tables the following results for the solubilities of the 
pure oxalates in water are obtained. 



t. 

0.78 
- 1.49 
- 2.50 

3.22 

- 5.88 



4-10 

20 


SOLUBILITY OF POTASSIUM OXALATE, KaCaO^Hi 

Gms. per roo Gms. Sat. Sol. Solid t9 Gms. per 


IN WATER. 

joo Gms. Sat. Sol. 


Soli 
pi., . 

CAQ 


CA 

2.48 
3-99 
5.15 
8.429 
8.83 
10,48 
11-57 


1.71 
3.20 
5-20 
6.705 

II.O1 

11.52 
13.69 
15.11 


KjCA. Phase. 
3-02 Ice 
5-68 " 
9.195 ' 
XI.855 " 
19-43 " 4K 2 CA.H 8 Q 
20.35 K.CA.HW) 
24.17 
26.675 


30 
40 

50 
60 
70 
80 
90.2 
106.2* 


12.36 
13.20 
14.14 
15.06 
15.94 
16.86 

17-73 
19.17 


16,14 
17.22 
18.46 
19.66 
20.8 1 

22.02 
23.14 
25.02 


28.50*' 1 
30.44 
32.60 
34.72 
36.75 
38.S75 
40,00 
44.19 



* b. pt. 

ioo gms. sat. aq. sol. contain 20,62 gms. K2C 2 4 at o, d 1.161. (Engcl, 1888.) 
The results oil Hartley, Drugman, Vlieland and Bourdillon (1913) and of 

Colani (1916), foi the solubility of nelitral potassium oxalate in water, agree 

satisfactorily with the above. 



SOLUBILITY OF POTASSIUM BIOXALATE, KHC*O, IN WATER. 

(Koppel aad Cahn, 1908.) 
. Gms. per ioo Gms, Sat. Sol. 



60 
102.4 b. pt. 



C 2 8 . 

8.75 
18.81 



KA 

6.50 

12.29 



Solid Phase. 
KHCA 



The KHC 2 04 is decomposed to the less soluble tetroxalate at temperatures 
below 50. 



K KALIUM 



744 



POTASSIUM Gobalii OXALATES, lacvo, 

K 3 [Co(C 1 04) J '|.IIjO and raoemic K s [ (!o( 0,O 4 3 13 l / IKO. 

SOLUBILITY OF EACH SEPARATELY JN WATKW. 
{J,3gr and Thorn**, 1918, mi!),) 

Gmx.raccmlr nail <;ni*. uvo salt 

t". i*r MK aw*. H,O. i" I 1 *** too gnu, 11,0. 

o 34*5*' -*>,. ........... l7...|o 

14 36.84 ^ **.... ^ 37.00 

By plotting these results the tran*ttion temperature is found to b< i3.a. 

SOLUBILITY OF MIXTURES OF POTASSIUM^ OXALATB AND OTHER SALTS ur 



Results at 15. 

Cms. per 105 Gms. Sat Sol 



Results at 50. 

Gmt. per 100 Om, St Sol SoUd Pfwse In 

10.03 ElaCa04+ 1 9*19 KC1 15*^ KtCsOi-f-^o.sfi KCl 

23.55 " 4" i.SaKtSOi 31.06 ** 4" x.w KS() 

20.39 (t H~ii6o ELNOs(i9) X9^J * -i'JH.jn^ K.NQ 

100 gms. aqueous solution, KmuitaneouHly mt united with |w>t;wsium and 
sodium oxaktes, contain 26.15 giro, K s CsO4 -r- 244 K N;i 2 CiC\ at 25**. 

tFwte wa*i Andrew, 1901), 

SOLUBILITY OF MIXTURES OP AMMONIUM OXALATX AMO or ^OTAitantM OXALATK 
IN WATER* f Hlvi*tt <tt<i (.)icu>RRr is it, i 



Results at 45". 
r too gmx/Mt. ftl, 



o.oo 5.oi 



.021 

,040 '^.67 47'^ 

.068 6.5i 438 

. I OS 1 2 . I O /|.OI 

.iaS i5.37 3.68 

.166 19.39 3.32 

.104 '4*3 *. 90 

25. ft 2,75 



Solid 



Solid t 



*lcf 

iftl, 1, 



.i3S 

,!54 

.187 



25. Q , . . , 

^6.S I .B3 ) ftftHit mitiiUon 

aft , 8 o . 8 5 > i n K, c, o* .1 i f 'o fin 



HenuliH it 50*. 



.10 



i I'h.is,-. 



) it! 



o.o 



,'454 3<M 4-7H (I)-*-(H) 
,u5*A HI. i o.o KfCjOi.HtO 



No evidence was obtainisd of the axiitnnee of n tlowbSn nalt. Tha proportion o! 
the two salts in the solid phases varing with the oompotiition of the flotation and the 
evidence is definite that mixed crystals of the twi> lira formod. 



SOLUBILITY OF POTASSIUM OXAI.ATS IN AQUKOUS SotuTioNH or SODIUM OXALATB 

AND VICE VKRSA 'AT ^5. (!Uvi*u imt U'Cunn^r, itnt.i 



Cnts, IMVJ- JtHt gm 

MH ; tot. 

</ of wt. nol. K s C a O,. N t II S 0, 

i.ai5 37.^ o.o 

1.218 a6.8 0.77 

1.223 a6,3 1.71 

i.aaC 26,-ji 4 js.i7 

i.aa8 26.1 a.5o 



it |fn 



Solid Ptoiw. 



/ f Ml. %lf 
.i; 
.IIS 

.oH-1 
.057 



, 1H1 3.71 



745 KAL1UM K 

POTASSIUM OX4LATE 

EQUILIBRIUM IN THE SYSTEM POTASSIUM OXALATE, NICKLE 
OXALATE AND WATER AT 30. 

(Vosburg, Israel ana Birch, lose.) 

The period of rotation was a week or more and special precautions 
were necessary to insure that the right solid phase was present. The 
oxalate content of the samples was determined by permanganate tit ration 
and the nickel content either by dimethyl glyoxime or cyanide titration 

Ons. per 100 Oms. per 100 

gps. sat. aol. SoUd gaa. set, sol. 8ollcl 

" 



2.26 0.08 SS 23.211 4.55 

3-77 0.55 " 25.82 4.67 

5.6? 0.57 " 26.83 4.93 

8.40 1.38 " 26.94 S.13 " 

ll.OS 2.55 '* 27.11 5.20 " 

12.44 3.53 II +V i(C ?4 ) 8 xH 2 3 - 55 S ' 8S 

14.22 3.80 K p NitC ? 4 L.xM 34.08 7-39 

16. 7 3.28 ' '" ' 33.03 6.64 " + KgC^.11,0 

18.77 3.48 " 33-31 6.81 

19-95 3-84 " 33*57 6.37 " " 

20.62 3.87 " 31-07 3-34 K j>W H * COO 

22.12 4-02 " 32.51 5.S6 " 

SS = Solid solutions of potassium and nickel oxalates. Analyses 
showed that water of crystallization in the double compound was most 
probably 4H ? 0. 

POTASSIUM Telluric Acid OXALATE 



SOLUBILITY IN WATER. (Rosenheim and Weinheber, 1910-11.) 

t o 20 30 40 ; 

Cms. K 2 [H 6 Te06.C204] per 100 gms. H 2 O 2.67 5.36 6.82 9, 07 1:2.35 



EQUILIBRIUM IK THI SYSTEM POTASSIUM OXALATR, ZINC OXALATK 
AND WATER AT 25. 

(Metier and Vostmrgh, 1933.) 

Qns. per 100 Oms. per 100 

0*8. sat, eol. *"* pm. mat. nol. *"< 



iCcToT znc.o ^ phaa<J /.^^..^^ PhMe 



3t.09 ii.il K ? C R 4 .II ? 1.1.7 13.71 4.86 2nC g 4 .3H ]B 

29.07 9-70 i.i.*7 11.73 3.85 " 

23.74 8.36 " 10.45 3-11 " 

21.17 7.63 " 9.44 2.59 H 

16.71 6.46 " 7.73 i76 " 

15.64 6.20 " 5.72 l.Oi " 

15.19 6.06 "* ZnC p 4 .2H g O 4.57 0,69 " 

14.26 5.80* " 3-80 0.38 " 

10.28 4.42* M 3.31 0.29 " 

* = Metastable, 1.1.7 " 



K KALIUM 



EQUILIBRIUM IK THE SYSTEM POTASSIUM OXALATB 
ZINC OXALATR AND WATKR AT 35 , 

(MitUur. ioa*.) 



35.96 


12.66 


K, 


35-66 


12.78 


l 


34.56 


12.77 




32.54 


13-02 


i 


30.07 


13.17 




28.33 


13.4 ) 




26.91 


13.68 




25.28 


13.70 





Gtea. ptr 100 8*8. m. ol. aolU 



( .H p O*i.i a :i , 99 11.65 ZnC f 4 .aHO 

21.48 to. 69 " 

19.11 8.94 " 

n.n a.Hs 

io,f>j *$. ; u " 

H.in 2.08 " 

5nC ^0 4 , aH f 5 , 36 o . 96 " 

3.14 0.17 fl 

1.1 = K g Zn(C^0 4 )^ 

Evidence was also obtained for the metasiabie existence of the com- 
pound K ? 55n^(C ? 4 ) j^.iaHJ) and the cofn(M>Hition of sirver.il 
solutions in contact with this compmind are givin 

coo 

BQOZtZBRZUM IN THB SVSTiM POTASSZWM OXALATl, 

OXALATX ANl> WATER AT 35, 



Tabular results are given for the temperatures 19, -|f/ 4il 53. 
Those at 19 yield a very irregular curve. Those at 35* A s/ "although 
giving somewhat better curves probably do not represent" equilibrium con- 
ditions, The following values taken from the 35 cyrv^ intlicati* 
roughly the general nature of the system. 

QM. ptrjMjpy.jiM.iol. Solid ft#. p r 100 . til, iui. 



12.0 trace K f O f O .H f O 2 ,g UICI ,. l-l( 

8 - 0.06 w a.8 I-aa ? 

2' - 3 S M 3 ,S i.ao ? 

6 --S 0.30 i.i.i.4<?) 2.0 0,92 3rC 

S' 0.38 l-s 0<?3 * W - 

*' '3 t * W l.O 0.60 

3>s -** 2 " 0.5 0.8 

30 0.80 " 



= K z C ? 4 .ZrO.C z 4 .H ? C/V,>H,.Ot?). 



747 KALIUM K 

POTASSIUM CHLORIDE KCL 

SOLUBILITY IN WATER. 

(Average curve from the results of Mcussor Z. anorg. Chem. 44, 79, VT, at 31.25, KShler - Z* 
Ver. Zuckerind. 47* 447. '07; Andrae J. pr. Chem. [a] 20, 456, '84; Gcrardin Ann. chim. phys. 
[4] 5t i37. *<5; de Coppet Ibid [5] 30* 411, '83; Etard lb%d. [7] 2,526, '94; Mulder; above 100, Tilden. 
and Shenstone Proc. Roy. Soc. (Lona.) 35, 345, '83.) 



^ Gms. KCI :per ioo Cms. 


Grm. KCI per ioo Cms. 


t0 Cms. 


KC1 per TOO 


Cms. 




Solution. 


Water. 




Solution 


Water. 


Solution. 


Water. 


~9 


19-3 


23 


9 


40 


28 


.6 


4O.O 


147 


41 


5 


70.8 


-4-5 


20. 6 


2 5 


9 


5 


29 


9 


42.6 


1 80 


43 


7 


77-5 


o 


21 .6 


27 


.6 


60 


31 


3 


45-5 


Solid Phase 


Ice 


5 


22.7 


29 


3 


70 


32 


.6 


48.3 


-9 


19 


3 


23-9 


10 


23-7 


31 


.0 


80 


33 


.8 


51.1 


-8 


I? 


7 


21. S 


*5 


24 5 


32 


4 


90 


35 


.1 


54-o 


-8 


16 


7 


20. o 


20 


25-4 


34 


o 


100 


36. 


.2 


56.7 


-7 


14 


9 


I7-S 


25 


26.2 


35 


5 


130 


39 


.8 


66.0 


-6 


13 


.6 


iS-7 


30 


27.1 


37 













-5-5 


12 


5 


14 3 



Sp. Gr. of solution sat. at o i.i5o; at 15 = 1.172. 

The following determinations of the solubility of potassium chloride in water, 
made with exceptional care, are reported by Berkeley (1904). 



to d of Cms. KCI per 100 * 
1 * Sat. Sol. Cms. H 2 O. * - 


d of Cms. KCI net 100 
Sat. Sol. Cms. H(). 


0.70 


I 


.1540 


28 


.29 


74 


.80 




I 


.2032 


49 


.58 


19-55 


I 


.1738 


34 


37 


39 


45 




I 


.2069 


S3 


38 


32.80 


I 


.1839 


38 


3 2 


108 


(b. 


pt.) 


I 


.2118 


58, 


.11 


S9-8S 


I 


.1980 


45 


.84 

















The following values for the Solubility of Potassium Chloride in Water 
were read from an average curve drawn through the more recent determina- 
tions of: Foote, 1927; Wright, 1927; Scott and Frazier, 1927; Malquori, 
1927* i928a; Flottmann, 1928; Cornec and Krombach, 1932; Lannung, 1934 
and Ilering, 1936. The values above 100* are the averages of the deter- 
minations of Cornec and Krombach, 1932; Achumow and Wassilijew, 1932, 
and Benrath, Gjedebo, Schiffers and Wunderlich, 1937. 

o d<of Ow. KCI per d.or (tat* KCI per 

sac. sol. 100 gins. sac. sol. sat. sol. too gnu. aau sol. 

-10.7 (Eutec.) 19.54 120 37.5 

o 1.154 21.92 130 1.235 38.4 

+ 5 22.9 140 39.3 

10 23.8 150 1.254 40.2 

15 24.7 160 nl.l 

20 1.174 25.5 170 1.276 42.0 

25 1.1778 26.4 180 43.0 

30 1.182 27.1 200 1.317 44.7 

40 1.189 28.6 Z2$ " 47-0 

50 1.194 30.0 250 49.3 

60 1.199 31.4 275 51.6 

70 1.203 32.7 300 54,0 

8 1-205 33-9 350 $8.6 

90 35.0 400 63.5 

100 1.210 36.0 454 69.0 



K KALIUM 748 



FRKB2IMC-POJNTS OF AQUIOUS SOLUTIONS OF POTASSIUM CHLORIDE. 
(B&rnta and Maaas, 1030.) 

The determinations sere made with the greatest possible accuracy. The 
temperatures of freezing are the averages of the point at which the 
first crystal of ice appeared and tfcat at which the last crystal disap- 
peared. 



OB*, KCl per Solid 0*a. KCl |Mr 
c 100 m** at >1. Ph*M & 100 pit. nu 01. Pbaat 

-2.24 4.9$ I< -10,31 19.03 Ice 

-.4.60 9.48 " -10,72 Eutec. 1^-93 " + KCl 

-6.88 13.70 " *2$.32 26.4* KCi 

THE SOLUBILITY OF POTASSIUM CHLOHIDE IH DEUTERIUM WATIH 
AND IN ORDINAKY WATBR* 

(Sneaman and Mnxua, 1997.) 

The deuterium water had a content of 98.3% f) f O and a density relative 
to that of ordinary water, of 1. 1059. The results are reported in moles 
of KCl per 1000 gms. of water ( = 55.51 ^oles \\ f O) md in 1111.7 gms. of 
deuterium water ( = $5.51 moles D^O). The same 0.4086 g. of KCl was 
employed in both solvents and the amount of deuterium water WAS 1,39 gm. 
The actual measurements were graphed and the following values for round 
temperatures obtained. 

Moles KC1 ptr.5ft.51 noltas Hol KCl pr 5B.Ht ol@i 



c 


'H |> 


V 


\f 


'v 


"' D t 





3.78 


3.16 


80 


6.80 


6.52 


10 


4*20 


1.68 


100 


7.51 


7" 2! $ 


20 


4.6l 


<t. 16 


120 


8*31 


7.97 


2$ 


4*80 


4.38 


140 


8.89 


8.67 


30 


5.00 


4.59 


l60 


9.57 


9.36 


40 


5.37 


5*01 


180 


10.24 


10.06 



60 6.09 5*79 



FREEZING-POINTS OF AQUEOUS SOLUTIONS or POTAKHIUM CHX.OKIDS. 

(Klein and Svanbrg t WJO, RwUbunh, ttlS.) 

Cm*. K.U Gm. KCt tim*. KCl 

t. per 100 co. ML wl. t*. rwf H gm. IMV t". pr loomJ. n,0. 

o.34 o.7<56(KandS) -3. 07,, 7.09 - c>.Hf... . .,. u*.6c) 

0.858... i.86.f -4.($<J... 10,77 - lo.Xj v'J.8o 



Data for equilibrium in the system potassium chloride * arsenic 
trioxide * water are given by Schreincmakers and de BAJU, 1915. 



749 KALIUM 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 
HYDROCHLORIC ACID AT o 

(Jeannel Compt. rend. 103, 381, '86; Engel Ann. chim. phys. [6] 13, 377, '88.) 



ram Alois. 


per 10 cc. 


Grams pf*r 


TOO cr. Solution. 


Sp Or. of 


KCl. 


MCI: 


ci. 


Htl. 


Solutions. 


34-5 


o.o 


2 5-73 


0.0 


I.I59 


30.41 


3-9 


22.69 


1.42 


I.I52 


27-95 


6.6 


20-84 


2-41 


I .150 


27-5 


7-i 


20.51 


2 -59 


I.I47 


2 3-75 


ii. i 


17.71 


4.05 


I.I37 


16.0 


23.0 


11-93 


3-39 


I. Ill 


IO.O 


34-o 


7.46 


12 .40 


I .105 


7-5 


41 .0 


5-6o 


14-95 


I . 105 


2.0 


65-5 


1-49 


23.88 


I .121 


2.4 


148.8 (sat.) 


I. S 2 


54-26 


I .224 



loo cc. saturated HCI solution dissolve 1.9 gins, KCl at 17. (l)ittc, 1881.) 

100 gms. sat. aq. HC1 solution dissolve 1.9 gms. KCl at 20. (Stolucnbcrg, 1912.) 
F.-pt. data for mixtures of KCl and HC1 are given by Dernby (1918). 
SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND OF SODIUM CHLORIDE 
IN AQUEOUS HYDROCHLORIC ACID SOLUTIONS AT 25. 

(Hicks, 1915.) 
Gms. per 100 Cms. Sat. Solutions. 



HC1. 


NaCl. 


KCl. 


O 


19-95 


10.90 


8.61 


10.65 


7-5S 


17.16 


3-56 


3 .8o 


20.65 


2.03 


2.86 


32.78 


O.l8 


1.27 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO- 
CHLORIC ACID AT AND AT 25. 
(Armstrong, Eyre, Hussey and Paddinson, 1907; Armstrong and Eyre, 1910-11.) 



Solvent, 
Gms. HC1 per 
looo Gms. H 2 0. 


Gms. KCl per 100 Gms 


. Sat. Sol. 


At o. 


At as*. 


O 


22.11 


26.45 


9.II 


20.93 


25.17 


18.22 


19.71 


24.07 


36-4S 


17.26 


21.74 


109.35 




13-47 


182.25 




6.93 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO- 

BROMIC ACID AND OF HYDROCHLORIC ACID AT 25. (Heir, 1911-12.) 

In Aq. HBr. In Aq. HCI. 

Millimolsper no cc. Gms. per Liter. Millimols per to cc. CSma. per Liter. 



HBr. 


KCl. ^ 


HBr. 


Kfl 


HCI. Klir 


' HCI. 


KCI; 


O 


42 


.72 


O 


^l8 


5 


5- 


,66 


37' 


49 


20.64 


279.6 


6.6l 


37. 


.80 


53-5 


28l 


9 


IO. 


,20 


33' 


70 


37- IQ 


252 


34:15 


19, 


57 


276.4 


146 




*5- 


,91 


28, 


,68 


S7-9& 


213.9 














20, 


-94 


24 


74 


76.35 


146.6 














32 


52 


17 


39 


118.6 


129.6 



KAL1UM 750 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS 
OF HYDROCHLORIC ACID AT 25. 



R 

Mai 


esults 
<iuori, 


of 
1928(0 






KVsu 1 


IS of 


Ingham 


19 * 


8 








Qns. pe 


- 100 


a ^ or 

<\ 




On. HoU. 


pr 


a 


5 or 


|H fc. M0U 




er 




pis. sat. 


$01. 


tat.. 


i 


000 cc ML 


. vol. 




nt. 


10CO ce ;ia 


c. 


sol. 


^Tu 


n 


_c_ A 


01. 


f 


fici" 


KCl *" A 




sol. 


^.^ru. 


~~~ 


<cn 


0. 





26. 31 


.1781 





.0 


4-199 


l. 


1169 


$^72 


0. 


607 


3' 


31 


20.93 


. 1671 





. 464 


3.7/18 


1. 


1372 


7 144 


0. 


309 


6. 


15 


15.87 


.1564 





.990 


3 . 3.8H 


1. 


1421 


8.un 


0. 


267 


10. 


31 


10.28 


.1467 


I 


.492 


a. 887 


l . 


1713 


10.68 


0. 


215 


is- 


07 


6-5* 


.1419 


I 


,8 13 


J.604 


i. 


1855 


11.74 


0. 


20 


23. 


15 


2.70 


. 1272 


2 


.74 \ 


K951 


I , 


l86l 


ll.8i 


0. 


22 


28. 


05 


1.87 


. 1 191 


"1 


.570 


l .449 


l . 


20O9 


13.96 


0. 


24 


31. 


83 


1. 19 


. 1 169 


4 


.008 


1 . 227 












40. 


98 


o. is 


.1150 


4 


.66*; 


0.96'^ 













IN THE SYSTEM POTASSIUM GKLO*ZDK, 

NITRATE, HYDROCHLORIC Aero, NITRIC ACIDS AKP WATBH. 



110 

130 
150 
170 
190 

210 
220 



110 
130 
150 
170 
190 
210 
220 



110 
130 
ISO 
170 
190 
210 
220 



Mo is. pr lOOO^tf 


a. reols, H 


F~ """'"'""" 


. -.-pr 


Results AI 


-20 


M.3 


106.7 


10.4 


117.8 


7.6 


127-3 


S.I 


114.7 


4.8 


141. 2 


6.7 


147-0 


8.7 


149.2 


Results at 


0* 


20, s 


104.0 


17.4 


104.7 


15.1 


123. 1 


14-a 


129.7 


14.6 


134.1 


16.7 


136,7 


20.0 


137.5 


Results at 


ai.s 


39. S 


104.5 


31.6 


111.6 


30.8 


117.7 


30.0 


122.5 


31.0 


136.0 


34.7 


128,2 


38.7 


128.7 



17.5 



40.4 
53-6 
69.7 

79.1 



36.1 
33.7 
42.0 
54*5 
70,5 
90.0 
103-5 



41.0 
53.0 

77.1 
95*0 

1*^0*0 



KCl 



75i KAtiUM 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS 
OF HYDROGEN PEROXIDE AT 25. 

(Ak.rlof end Turclc, 1935.) 



Composition of 
aq. solvent, in: 



percent Mol. Fraction^ 



Gta. Mo la. KCl 

dissolved per 

1000 8W. solvent, ' 



Composition of 
aq. solvent In: 

" 



On. Hols. KOI 
dissolved p@r 



" MoTT F r acHotT^ 1000 as solvent 



0.0 

5.30 

10.73 
15.72 



0.0 

0.0288 
O.OS99 
0.0899 



4- 826 
4.835 
4.974 
5-093 



21.19 0. 1270 
26.24 0.1585 
31.43 0.1955 



5.263 
5.362 
5.534 



SOLUBILITY op POTASSIUM CHLORIDE IN AQUBOUS SOLUTIONS 
OF POTASSIUM CHLORATE AND VICE VERSA. 

(FltcK., 1937.) 



Gam. per too gns. sat. sol. 



Results at o 



Solid 
Phase 



ouof QJBS. P er JLOO^. sat. ol. 
sat. sol. / ""~iccr~ KCIO "* 



Solid 



Results at 40 



1 


.153 


21 , 


90 


0. 


,0 


KCl i 


.188 


28.7$ 





.0 


KCl 


1 


.157 


21. 


,16 


0.71 


w * KCIO. i 


. 196 


27.74 


i 


.54 


" 


1 


.121 


16.21 


0. 


82 


KCIO^ ' i 


.206 


26.49 


3 


.15 


"4 KCIO, 


1 


.068 


8. 


47 


1, 


09 


i 


.165 


20.66 


3 


.88 


KC10 B 


1 


.022 


0. 





3- 


OS 


" i 


.148 


18.43 


4, 


30 


" 














i 


.116 


13. 16 


s 


.44 





Results 


at 20 


i 


. 106 


10.76 


6 


.39 


" 














i 


.098 


8.71 


7 


.25 


it 


i 


.176 


25- 


70 


0. 





KCl i 


.092 


7.66 


7 


.64 





i 


.183 


25. 


17 


0. 


89 


" i 


.084 


4.60 


9 


.20 


H 


i 


.184 


24. 


60 


1. 


55 


" * KC10 3 1 


.074 


0.0 


11 


.65 


n 


(i 


.177 


25. 





1 . 


56 


" " " ) 












i 


.153 


20. 


26 


1 . 


75 


KC10 3 




Results 


at 50 






i 


. 106 


13- 


47 


2. 


44 















i 


.070 


7. 


44 


3. 


74 


" i 


. 194 


30. 18 





.0 


KCl 


i 


.051 


2. 


84 


5- 


18 


" i 


.207 


28.24 


3 


.27 


K 


i 


.044 


0. 





6. 


78 


" i 


.214 


27.45 


4 


.46 


" 4 KCl 0, 














(i 


.211 


28.3 


4 


-32 


it it *j 


Results 


at 30 




i 


. 155 


18.53 


5 


.76 


KClOg 














i 


. 147 


17. SS 


6 


.01 


M 


i 


.182 


27. 


30 


0. 





KCl i 


.105 


8.51 


9 


.66 


II 


i 


. 190 


26. 


64 


0, 


87 


" i 


.088 


0.0 


14 


,76 


H 


i 


.198 


25. 


81 


2. 


29 


" * KCIO. 












i 


. 140 


17. 


86 


3- 


12 


KCIO,, 




Results 


at 75 






i 


.108 


13. 


06 


3- 


82 


11 












i 


.097 


11. 


03 


4. 


38 


(i 


.244 


29.30 


8 


.08 


KCl* KC1Q,) 


i 


.088 


9. 


45 


4. 


82 


" 

















4. 


67 


6. 


62 


" 


The 


three determinations 


in parfn- 


i 


.058 


0, 





9. 


24 


" theses are by 


Donald, 1937. 



C3 



A series of determinations for this system at 20 are reported by 
DiCapua and Scaletti, 1927, but differ considerably from the above re- 
sults and are probably incorrect. These authors also give results for 
the equilibrium in the system KCl + NaClO_=to NaCI * KCIO, at 20. 



KALIUM 752 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUKDUS SOLUTIONS 
op POTASSIUM CHRQHATE, BICHROMATE AND PEKHANGANATE AT 25. 

(Her?, and Hlobern.mil, i'.);>o.) 



Results for aqueous solutions of: 
Potassium Chromate 

Qa. Mola. jper 11 ur OR. Hola.^tr llttr 
'K-Croj- IccIP 'xjtrtl'/ """xcT ^ 

c 1 c r y 6 



Potassium Dichroroate Potassium 

Permanganate 



fl*. Kola.,. 



KC1 



KC1 



0.0 


4.19 


1-73 


3.61 


0.04 


4. IS 


o.o 


4*19 


0.4 


4.01 


3.11 


3.47 


0.08 


4* 12 


0. 05 


4.02 


0.8 


3-87 


2.S7 


3-33 


O.l6 


4 10 


o.n 


4*04 


1.28 


3-74 


+ 4.69 


2.69 


+0.38 


4.05 


4-0.40 


4.00 



SOLUBILITY OF PoTASsiim CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM 

IODIDE AT 25 AND VICE VERSA. 

(Amadbri and JPamjwmni, itjn.) 



Gms. per 100 Cms. H^C). 



KG. 
O 
4.06 
7^3 
11.36 


KL ' 
149 . 26 
144.03 

W-79 

132.60 


11.74 


I33-90 


I5.IO 


105.^1 



<jm.__pff too (5mi, 



KC1, 


KL ' 


19.64 


68.22 


2 37S 


43.89 


29.56 


23.% 


3^3 


14.83 


33-68 


7 


36.12 


o 



SOLUBILITY OF POTASSIUM OtLoiu&t IN AQIIXOUS SOLUTIONS or 
POTASSIUM Ioig ANO Vici VISA AT SIVIKAL TIN^BKATUKBS* 



Results at 20 



(tea. par lOOcc 
sat, ao^itlon 
KCl KI 

0.0 
90.7 
92-3 
95-3 
97.4 
100.3 



Solid 



29.74 
6.69 
5. OS 
3.47 
1.82 
0.0 



KC1 



KI 



(Harris etnd OhrioUmiaen, 

Results at 30 

(taa. per 100 ec 



KGi 
" * 

KI 



31.88 
7.84 

5-53 

4.21 

2.03 
0.78 



0,0 

92.9 
96.8 

98. o 

100.4 

103.2 



KI 



Results at 40 


(tea, per IDC'CC 


JSL.3 


Jutlon 


Solid 




. ~j~\ 


PtUMW 


33.98 


0.0 


KCl 


7.36 


9S-9 


H , I 


5-55 


97*9 


11 


4.39 


101.2 


It 


2.04 


104-5 


n 


0,0 


107.3 


t* 



SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM 

IODIDE IN WATER. 

(Kurd Ann. chim. pfap. [7] j, 375* '04.) 

Gmmt per too Cms. Solution. 



a Grams per 100 Cms. Solutiaa, 




KCl. 


tfi. 




O 


3-7 


50-5 


100 


2O 


4.2 


53-o 


140 


40 


4-7 


55 -3 


180 


60 


5-2 


57-5 


220 


80 


5-7 


59-4 


^45 



KCL 
6.2 

7-3 
9.4 

IO-O 



1CL 

61 .o 
63 . 7 

65 5 

663 
66.5 



753 KALIUM 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM 
NITRATE, AND OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF POTASSIUM 
CHLORIDE, AT SEVERAL TEMPERATURES. 

(Touren, 1900; BodlUnder, 1891; Nicol, 1891; Soch, 1898.) 



14-5 (TO- 

Gms. per Liter Solution. 



KN0 3 . 

O 

20.64 
32.18 
62.23 
82.77 
II5.9 

123.4 



KCI 
288.3 
284.2 
282.1 
276.8 

273-5 
270.7 
268.3 
267.2 



KCI in Aq. KNOa Solutions at: 
25.2 (T.). 

Gms. per Liter Solution. 



KNOa. 

O 

13.76 
32.18 
91 .26 
122.7 
I4I.4 
182.7 



KCI. 
3II.8 
306.6 

303-<> 
293.2 
287.2 
284.2 
276 



20, etc. (NO- 

Gms. per 1000 Gran. HgO. 
' KN0 3 . " KCI. 

o 345-2 

56.18 342.15 

168.54 334.39 

at 25 (S) 
225.8 341.3 

at 80 (S) 
1175 402 



14-5. 

Gms. per Liter Solution. 



KCI. 


KNO,. 


O 


225.4 


13-58 


219.8 




208.2 


65.64 


185.2 


132.6 


159-5 


164.4 


153-3 


196.5 


144 


236.9 


I37.I 



KNOi in Aq. KCI Solutions at: 
25-2. 

Grns. per Liter Solution. 



KCI. 

19-39 
49.22 
IOO-7 

I5S- 2 
207.3 
226.8 



KNO 3 . 

3*2-3 

288.7 

254 
224.4 
203.9 
196.9 



20". 

Gms. per 1000 Gms. HgQ. 



KCI. 
O 

82.9 
165.8 
248.7 
310.8 



KNO 3 . 
3II.I 
256.8 
221 .7 
2O2 
501.6 



In the case of the results by Touren, constant temperature and agitation were 
employed. 



KCI. 

O 

4.72 

7.74 
12.23 



KN0 8 in Aq. KCI at 20.5- (B.). KCI in Aq. KNO 3 at 17.5 (BO- 

Gms. per 100 cc. Solution. Sp. Gr. of 

KNOa< ' Solutions. 

27 68 1.1625 

24.39 I.I700 

22.44 1.1765 

20.23 I.I895 

18.96 LI933 

T9.6i 17.67 1.2150 

22.17 17.11 1.2265 

24.96 16.79 1.2400 

In the case of the above results by Bodlander, a saturated aqueous solution of 
potassium chloride was prepared and weighed amounts of potassium nitrate were 
added to measured volumes of it. The mixtures were warmed and then allowed 
to cool to the indicated temperature and frequently shaken during 24 hours. 



Gms. per 100 cc. 


Solution. 


Sp. Gr, of 

Solutions, 


KN0 3 . 


KCI. 


O 


29-39 


I.I730 


6. 5 8 


27.50 


X.I980 


8.88 


27-34 


I. 2100 


12.48 


26.53 


I .225O 


14-83 


25.98 


I . 2360 


15 .22 


25.96 


I . 2300 


15-49 


25-95 


1.2388 


15-33 


26.24 


I.24IO 



K KALIUM 



ci 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIOKS 
OF POTASSIUM IODATB AND Vies 
(Hill and Rlccl, usi.) 



d. or 
sac. sol. 


Ctas. per 100 tjas. sat. soi. Solid 


d.of Oto*. Pr 100 t 

sat. sol. r"~~KT5^ 


jpc. sat. sol. Solid 
"" kri "" phase 


' KID,, 


KCI 


m 




Results at 


5 




Resu 1 1 s at 


25 ICon.) 


1-15S 


0.0 


22.84 


KCI 


1.073 429 


5.9 * KIO, 


1. 170 


1./J4 


22.64 


" + KID, 


1 , 066 5.83 


.!.?H * 


1.U7 


1-50 


19.56 


KIO, 


1,071 H.45 


. " 


i . 08*1 


1.79 


10, 13 


n 






1.044 


2.91 


3-03 


It 


Results at 


50 


1-043 


5.16 


0.0 


II 


* o . o 


30. o^ KCI 










1.77 


jjt).qo " 




Results at 


25 




~~ 3.07 


?9.o8 "* KIC 


\.179 


0.0 


26.36 


KCI 


3,7 ?{ 


a*. 17 KIO 


1. 1^7 


2.10 


25.82 


" * KIO 


4.71 


H.6i| M 


1.153 


2.40 


19.64 


KIO 


7 . n :-? 


6.83 


1.109 


3-01 


12.37 


H 


- 13.31 


. 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUKOUS SOLUTIONS OF 

NlTRATK AT O AND AT ^5. 
(AnnHtrotu; am! Kyrr, ito- n .) 

(ms. KCI DitsolvTil ner 
TO (nv Sit!, Sl, it ion nl 



Solvent, Cms, 
per 1000 Urns. 
H 2 0. 



22.10 



O 

25.27 

50.55 
IOI . 1 I 

151.66 

SOLUBILITY OF POTASSIUM CHLORIDK IN AQtiEOtis SOLUTIONS 

NlTRATK AND VlC'K VERSA, 

(Leather arid Mukcrji, i 



2! ,25 
20,70 



26.73 

26 . 26 
25.61 
24.58 

M-57 



POTASSIUM 



Sp. Gr. 

<sa t <srtl 


Results at 30. 

Cms. per 100 Gnw. 
HA 


Sp, Gr. 
Sat Sol 


Results at 40. 

(tnw. per ipo (ms. 


Sp, Or. 

C a * C fl ) 


Result* at 91. 

(Jms. }wr jc *,!, StiHd Phase 
H-.U, j n 


oil 1. DOI< 


"KCI. 


KNO a . 




KCI. 


KN() a . 


.iftCt 7<I 


KCI. 


KNO<, t'.^i'h Case. 


I 


.186 


37-S 





I 


.194 


40.60 


O 


1.222 


53*5^ 


O 


KCI 


I 


.219 


3^-72 


3.05 


I 


.252 


39-" 


16.86 


1. 344 


47,85 


Si. 


.75 " 


I 


.251 


36.IQ 


10.36 


I 


.305 


37.o8 


3545 


1.486 


43. jo 


114, 


,6 


I 


.281 


35-42 


26.83 


I 


310 


3740 


30-7' 


1.552 


30.00 


i6a, 


,0 " fKNO, 


I 


.258 


28.71 


29.19 


I 


.312 


32.22 


41.52 


1*544 


33. j 5 


165, 


,6 KNO, 


I 


.241 


19-35 


32.34 


I 


.207 


22.6$ 


46.^1 


1-545 


15.56 


fHi, 


,1 " 


I 


.225 


944 


38.10 


1 


.270 


JI.58 


52.66 




o 


202, 


,H 



Results are also jfivcn for ao. 
SOLUBILITY OF POTASSIUM CHLORIDE IN Acit'F.oimSoLti'noNs or POTASSIUM NITRATE 

AND VICE VEBSA AT 30. (Ilftrhaudy, SM3. i 
(Jns. pur 100 gins. bat. sol, (*mn, j>rr iiu fnit %ni <>) 

^ "" 

KCI. 



22.78 

;,2.iH 

21 .CJ 

Data 
water at 



KN0 3 . 
0.0 

1 3 4* 
l6.3() 



Solui 



KCI 



AO . u > 
10. 48 

MS 

o.O 



KNO,. 



Hi .4 



KNO, 



{or equilibrium in the system potassium chloride -}- potaHKiurn oxalatc + 
t 20 are given by Trifuov, 197.4-197 5. 



755 



KALIUM K 



SOLUBILITY OP POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM NITRATE AND VICB VBHSA AT 18.5. 

(Holluta and Mautner, 19P7.) 

To standard solutions of one of the salts an excess of the other salt 
was added and the mixtures heated to 60 and then cooled and shaken at 
18.5 until eguilibrium was attained. A given volume of the saturated 
solution was evaporated to dryness and from ^ e ^ Q \jJ^l^^ tn residue, 
the concentration of the original aq.. solvent . ana^oT^ the original sol- 
vent and the final saturated solution, the weight of each salt present 
in looocc of the saturated solution was calculated. The results thus 
obtained agreed satisfactorily with calculations based upon chloride 
determinations. 



Qra. Mols. KN0 3 
per liter 
aq. solvent; 



d. or 

sac.. 
sol. 



QMS. per 1000 cc 

sat. solution 
/ _-_^-^_ v 



Oo. MOU. KC1 

pr liter 

aq. solvent 



d-of 

sat. 
sol. 



Gtas. per 1000 cc 
aat. solution 



0.0 


1.1738 


o.o 298.50 


0.2 


1. 1820 


17.74 294.84 


0.4 


1. 1899 


35.46 292.32 


0.6 


1.1985 


53.28 288.86 


1.0 


1. 2147 


88.86 283.16 


1.5 


1.2348 


133.66 274.62 


1.6671 


1.2415 


148.84 271.24 



0.0 
0.2 
0.4 

0.6 

1.0 

2.0261 
3.0025 
3.8975 3 


. 1560 o.o 265.92 
. 1573 13.36 254.64 
. 1598 26.80 245.84 
.1621 40.38 235.66 
. 1682 67.76 218.96 
. 1887 139. 16 184.74 
.2141 207.94 163.74 

L.241S 271.24 148.82 



SOLUBILITY OF POTASSIUM CHLORIDE IH AQUEOUS SOLUTIONS 
OF POTASSIUM NITRATE AND VICK VERSA AT 25. 



Cl 



Qms. per 100 fpna* sat. aoi. 



Solid 

Phase 



26.5 

25.05 

23.75 

22.95 
21.94 



0.0 

7.92 
11,41 
14.72 



KC1 



KNO W 



per 100 HJMS. aat. sol. 

""""" ~---^ -v 

17.20 
19.82 
22.30 

24-02 
27.86 




KNO, 



Results are also given for the effect upon the above equilibrium of 
the presence of varying concentrations of HC1 and of KOH. 

The following values for the simultaneous solubility of KG! + KNO^ 
in water at other temperatures than 25 are also given by Nikalajew", 
1929- 



Gats, per 100 gm. sat. sol. 



KCl 

0.2 20 . 44 

17.0 22.23 

40.0 21.28 



Solid 

Phase 



Gets. p@r 100 gpa. MX, 0ol. 
^___~. --j^^--" ~\ 



Solid 



6.38 
1 1 . 00 

21.98 



KC1 



60 

Bo 

100 



18.56 
15-^7 
14.96 



34.12 KCl 
46 . 29 " 
53.88 " 



K KAL1UM 



OF 



d, of > 0t. per 100 pu. 

*t. *oi. '-nKr-^iwi 






Results at 



M .it 



27.9 


0.10 


KCl 


27.7 


8.7* 


11 4 KNO 


o.o 


13.3 


KWO^ 


Results 


at 35^ 




*-m 35.9 


0,0 


KCl 


*'*38 34.8 


16.3 




^^i 34-5 




w * KNO, 


1-256 32.8 


31-1 




1*313 IS- 9 


38,0 


M * 


1.197 8.0 


12. a 


H 


1.189 o.o 


38.1 


H 


Results 


At 50 




J94 42.4 


o.o 


KC:I 


350 38,3 


54,1 


1 * KHO, 


-333 13-7 


61.3 




329 n.9 


71*5 


H * 


33^ 0.0 


85.7 


tt 


Additional res 


wits for 


this wstM 


id 32Q i t^rw 


i of th* 


nyli^r of " 



, JO I 

. 1 1ll 

. -j88 



IIKJ 



H. J 
0.0 



IKtl 

to.H 

7J.7 
M 1 . 

IJ3.0 



AC 100 
0*0 

65,0 



3K>9 . 

J3II.CI 
JiJfl.O 



KCl 

KNO R ! 

KCl 
* t KMO. 



-.' 



a. or 

*t- Ml. 



DM. 



35 


2SJ 


3*1-9 




.336 


14*5 




.266 




SO 

7S 

n 


353 


37*6 
46.6 




393 


11.8 




461 


19.1 


00 


-573 


39.8 



"'-'* 

35. 8a 
31.22 
12.57 



23,1 
16*7 

408 
72.9 



23.84 
13.48 

21.66 
19.7? 









1.15 



KCl 
KCl 



til 



3.08 
i.fi 
i ,80 
1.77 

1,86 



KKO, 



KNO. 



0.70 KCl * KVO. 



3.66 



KNO. 



757 KALIUM 

EQUILIBRIUM IN SYSTEMS COMPOSED OF POTASSIUM AND SODIUM CHLORIDBS 

NITRATES AND SULFATIS. 

Complete experimental data, including densities, in the form of tabu- 
lar results and diagrams for these complex systems at temperatures be- 
tween o' and 90 are given by Cornec and Krombach, 1929, and Corr^ec, 
Krombach and Spack, 1930. These authors have made use, when necessary, 
of the results for the ternary and quarternary systems previously re- 
ported from their own laboratory and by other workers, including, 
Chretien, 1929, Cornec and Bering, 1925-71 Comec and Krombach, 1929* 
Meyerhoffer and Saunders, 1899, d'Ans, 1915 and Blasdale, 1918. 



NH 4 C1 at -10 



and -1 



Equilibrium in the Reciprocal Salt Pair 
KC1 -* NH 4 N0 8 3 KN 

( (Krl cache wsKy and Ooldnann, 1954.) 

These results supplement the previous determinations of Janecke, 
1928, at 0-80 and Aronawa and Lunskaja, 1933, at 100. 



Results at -15 



Results at- -10 



Oto. 


Mola. per 


JLOOO as. V 


Gta. 


MO la. per 


1000 0ns. 


HQ 


Solid 




' KCl 


MH 4 C1 




KNO_ 
o 


NH 4 N0 3 ^ 


' 


TKF"" 


"~~M^IL 


_^ 
o 


43 


Phase 




1.64 


4.11 










1 


.60. 


4.15 








KCl + NH 4 


Cl 





3-79 







7.67 







3.99 





9.l6 


Nil Cl -f NH 













.892 


10.33 










1.04 


11.96 


KNu.. - " 















_ 


2 


45 


1.91 





_ 


KCl 





















.661 


4.63 








NH 4 C1 


















1 


.38 


4. 48 


0.502 


. 


"% KCl 




0.976 


4.35 





774 





1 




4-59 


0.921 


n + + KNO. 





3-90 





.890 


8.28 




. 


3.99 


0.900 


9.49 


NH 4 C1 + NHJ 


m 



SOLUBILITY DATA FOR THE RECIPROCAL SALT PAIRS KCl+NaNOa^NaCl+KNOs 

AT 5, 25, 50 AND 100. 
(Reindm, 191:4, 1915; see also Uyeda, 1909-10.) 



Results at 25. 



Results at 50. 



Cms, per 100 Gms. H/). 


Gms. per 100 Gms. H/). 


Solid Phase in Each 

Case. 

NaCl 

NaCl+KCl 
KCl 

KC1+KNO 3 

KNOa 

KN0 8 -HNaNO 3 
NaNO, 

NaNOa+NaCl 
NaCl 
NaCl-HKCl 
KCl + KNO, 
KNQi+NaNOa 
NaNO,+NaCl 
NaCl+NaNOa+KNOj, 
NaCl+KCl+KNOa 


NaCl. KCl. 
36.04 
32.28 10 
30.27 16.45 
12 26.78 

35-54 
... 34.92 

10 
IO ... 

23.62 
33.90 

24.82 22.2 
21.36 2O 
24-5 

7 

2 3 .8 
4.5 


NaNOa. 

IO 

60 

100.9 
96.06 

77.46 
58.01 

10 

15-4 

6V/3 
82.1 
64 


KN0 3 . 

10 

22,79 
31.48 
37-49 
41.87 
46.15 
20 

32.9 
17.2 

43-iS 
41.2 

40.3 


NaCl. 
36.72 


KCl. NaN0 3 . 


KNO a . 


28,35 


23.09 .. 
42.80 
41.39 ., 
38.75 - 


24.05 
52.54 
85.10 



















... 134. 
... 114. 


9 
i 


90. 


2 


20. 

28. 

34 

12, 


5 
4 

7 


... 84.8 
... 43-9 
13.4 
25.4 


24, 
5*. 


.6 


19- 

12, 

59 


,2 

.2 

9 


... 104 
no 
6 


.1 

7 
. i 


27, 
82, 
70, 


,2 
,2 

9 



Results at 5*. 



31.50 



27.6 



10.4 
29.84 



82.10 
41.7 



10.14 
18.1 



Results at 100. 
27.3 36.2 

41.6 ... 199 

233.6 218 

19.2 ... 158 



NaCl-t-KCl 



KNOj+NuNOj 
NaNOrf-NuCl 



K 



K KALI DM 758 



Cl 



POTASSIUM HYDROXIDE AT VAHIOI'S '!Y.Mi*F!tATriit>:a. -v*m Aitt^Hii 


or 


Cms. K OH 


<im< KUIMT m, ,,i w noi, 




per lOOflms. 
sat, sol. 


-SIM. -in, ! * !> "" 


ao*. 


5 


1 5,,|i f . I So't 1 7/n I , I H Vt i <j.uu 1 , 1 84 t a<>.8< i . i Ho) 


aa.u(u8a) 


10 


11,711.1%! i.'i.u i.i<j.|t i'.fn i,-o'ii il,.|i i ,'*fti i 


17.9(1.204) 


i5 


7,t}( f ,'Mj/j ) 8.81 I /'tit* j.jt' i /.* ii| i f i .'!' i .-*'- > i a, If i .->',* 6 i 


s3.f>(i,23o) 


o 


5 6( I ,a3o/) tf.'lt I .*i'l8 i -.'*' I .* $*| 8,01 I .. if 1 1 8.H< I ,-,*, V* ^ 




25 


3.(i(i.v.8o') <.l i,'i;'H"l 4.o,u/jH'ii ->..{< l .^8 f > Icii'i/iKli 


7.4(1.289) 


3o 


v,.Xi.3r> v,tid/h'l> 'i.o(i.377i 3,l*i! i;i*Ji :|,',! i.'liH) 


5. 0(1.3*3) 


35 


1,2(1,376) I/(l.37'0 1.811.370) /.*! i.iitiu ;t.lk !.3chl 


3.a( 1.364) 


4o 


o7( i { 3o 1 O.OA i 4 > "> i i .< i . -i i tl J < M 4 | * 4 * "M i ..I t s 1 


1,8(1,409) 


45 


o.4( I .<JK6l </H S ,,{78 1 CJ/H. i ,47 f ' f "v 1 ! - I f "J ' "'W, ! "P" 1 '^ f 


1.1(1.460) 


5<> 


o.'ii'i/* * r i i fijlf l,*ni 1 


o.8(i.5i5) 


55 





0.5(1.571) 


Gmi. K Oil 


(imt. KCl IMT u smt C t Ulmi ..i 




pftr 100 |f ins, 
sat, .Mil, 


,,ll", ,", '>*>* 1 "* ' l.0* 


ir. 


5 


7,4,7 U*lHli) '; . 1 C*i . Itjli) *><|.'; ( I , ;l |f Vi.o 3<i, 


38.3 


1C) 


v.o.a(i.'>oHy 7'A.7(i.r4i>1 /l.tttf ,'iln ^:,*i 'to.H 


33,1 


i5 


i6.o(i.u36) iH ,|i$.^4*^ O.OM.?M> *a.<> 4 *KH 


'j8.i 


ao 


17.3(1.7,63) M.4<i.)7<n i>.jM.v7v i8.< vi.- 


i3. 


a5 


9.1(1. 'M\,\ I i f > . H ( t . '/i 19 i i v . i u '/<jK t i i , f i i ; , o 


19.1 


So- 


6.3{i.34) 7,7li,:i3ti| *|, i ii ,Ttii n/l ii.8 


15.3 


SS 


4,1(1.3)8) r *. 3d. 364) fJili iti; H.8 i/i 


ri, i 


4o 


a . 5 { i . 44 > 3.711, jo. 4 1 4 * ' ! * 48 t > . ; Ho 


9.3 


45 


1.6(1.458} ^. r >n.4*>n l,iii,4*i ,o f.o 


7-< 


5o 


l.l(l.Stl) I.7(l,fH4l ..U.HKU "1,1 /| 8 ,f 


5 5 


55 


0.9(1. 56H) r , i ( i . flfiiVl i , H ( t . >Mi i '* , f H * i 


4-7 


60 


s . i 1 1 . ft i H i , o a . 7 


4.0 


65 


1,7 "^, f i 


3.9 



70 .- 7.7 

Th figures in parentheses ar lli tienstttm of th iatiiratfti Holutious. 
SIMULTANEOUS SOLUBILITY OF POTASSIUM iii.oiop A NO I'OTAHMI'M HYDHOXIDB 

AT THE EUTKCTIC TlCMPKHATU fvn 4ttlrt|lf tU4.J 





Cms. par W gm. 




tm% fwr i IWH- 




Ml. iOl 




<%!, *t. 


Eutec, 


' '**' s ****,^%, - *w^'*' * 


4illit F.uirr. 


f "*,,, - ,***- 


tt'iup. 


KOH. KCl. 


l*br, t<*m|t. 


KOH. WU. 


!4I.30 


1 1 . '>, 3 9 . % 


M:I r, . *i> 


jH , l|*| f'i, || 


17.3) 


10.6* io.a<j 


lii 


*nji| o. i > 


- H . O 


HJ.?4 


V 


1 , 8'i C 1 1 


67. -A 


30.73 0.'>.3 K< 


.>H.m,0..f.-ttn* lit) 


'*'.78 0,47 


65. a 


3o.83 


> Ml 


*>8 4 ot 0.1*7 


65.6 


/9.6-js 


> *tl 


*><|Ji*i o.i)l 


64,3 


3o.59 0.43 


-*-K:I *jo 


l.7' I .V'l 


21.3 


46.6 o.38 KJ 


Ittf 1H,0 -Kf.| 1 AO 


(>5.3t i .7** 


n. i 


47-45 <>.38 


1 .10 


73.f7 ^.87 



KOH. 11,0 t 



KAL1UM K 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 
POTASSIUM HYDROXIDE AT 20. (Bronstod, 1920</.) 

Gm. mols. per liter. (Jm. mols. per lltor. Gm. mols. per lller. 




KOH. 
I I . I O 

*'-* I( J 
1 ?. . ()'A 

13.84 



0.191 

0.168 

o.i 38 



KOH. 
1 4 . 0:>, 
I/I. 85 
I.). O2 




SOLUBILITY OF POTASSIUM CHLORIPB IK AO.UBOUS SOLUTIONS 
OP POTASSIUM HYDROXIDE AT 25. 
(Attrlof and Short. 19^7.) 



0m. Mols. per 


Gnu Mols. per 


On. Mols. 
1000 &%*. 


per 

M^ 


On. Mols. per 

1000 . MpP 

i^~------^--~rr~ >. 


' KOH 


KCI x 


/KQlif 


KCI > 


/- 


K 


1 


KCI 


' KOH 


KCI ' 


1.023 


4. 


079 


4 


.102 


2.265 


8. 


37 





.894 


15-53 


0.28l 


1.053 


4. 


056 


5 


,187 


1.847 


9. 


43 





.750 


16.59 


0,247 


2.033 




397 


5 


.273 


1.839 


10. 


54 





-638 


18.42 


0.210 


2.126 


3* 


365 


6 


.108 


1.444 


11. 


28 





529 


19.32 


0.198 


2.897 


2. 


889 


6 


.203 


1.576 


12. 


S3 





.433 


20.64 


0.183 


3.150 


2. 


778 


7 


.210 


1 . 246 


13- 


42 





370 


20-55 


O.l84 


3.998 


2. 


473 


7 


.211 


1.175 


14. 


44 





.311 







Cl 



It. pt. 



//of 

.Ht. S(t|. 



Cms. per 100 gins. sal. sol. 



The solid phase is KCI in all cases. 

SOLUBILITY OP POTASSIUM CHLOEUDK IN AQUEOUS SOLUTIONS 
OF POTASSIUM HYDROXIDE AT THE BOILING POINTS, (von Autropoff, 102'*. 

Grns. per 1 00 KIUH, *l. ol. 
KOH. 
0.0 

5.0 

4o.o 

,15.0 



KCI. 



II, pi. 

I vio . 7 



ROH, 



KCI. 



109.2 
1 10 

HI. 5 

u'J.5 



r . 



.320 



22.9 

18.7 



i:j y .:j 

i ' n . 5 



r >5,o 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUBOUS SOLUTIONS 
OF MONO POTASSIUM PHOSPHATE AND VICB VKRSA AT o. 

(Aokunaay and Nssl@r, 19W.) 

The results are expressed in the Janecke method which is in terms of 
the number of gm. mols. of H p O required to dissolve 100 gm. mols. of 
salt or salt mixture of determined molecular composition. 



1.9 
9.6 

7-7 
6.4 
5-4 
4-7 



d. of 
sac. sol. 



.1690 
.17SO 



1199 

.1183 

.1179 

1.H58 

1.1151 



Cojnpoal clon 


of Dlsaol 
On. Hola. 


KCI 


v^ 


100.0 


0.0 


95-8 


4.2 


92.1 


7.9 


73-0 
62.7 


27.0 
37-3 


44.9 
31-7 
18.1 


55-1 
68.3 
81.9 


0.0 


100.0 



OB, Mols. H ? to dloXv tOO 
g. fitola. aalc mixture 



Solid 



2210 
2860 
3320 
3540 
4125 



KCI 



" * K!LP0 4 
KH J> P0 4 



The author also gives results for the quarternary system (K, NH ) 
(Cl r H 8 P0 4 + H g O at o. 



K KALIUM 



760 



d.or 



SOWBXUTT OF POTASSIUM CHLOIS IN 

OF POTASSIUM SOLAH AW VICE V**** 



Result* 



Results at o 



( COIU) 





_ 



I 
7 


.0 

.08 
.38 


27 

a7 




9 KCl j. l04 

.0 K,SO f " 4 


^5 o.o K f SC 

Results at 75* 


Results at 25 


203 


0: 


.0 


^ 


.6 


KCl 


i 
i 
i 
i 


.179 
.185 
153 

.120 
.092 



1 
2 
3 

6, 




45 

13 

40 
07 


35.9 KCl 

35^7 " * K 80 

V QA * 
27,1 A F J 4 

18.2 " 

9.2 " 


.211 
-171 
135 
. 1 10 

n6 


a, 14 
1.46 
5.82 
10,8 
ao.fi 


ti8 

16 




*8 

l 

. 


K J5T 




i 


.086 


12. 


1 


0. 


" 


Hesw? is 


at it 


)0 




Results 


at 50 
























2.311 


0. 





55-5 


KCl 


i 
i 


194 
200 


0. 
1. 



70 


43. 

42. 


o KCI ^ J;JIJ 


3. 
31*. 


55 




SS- 

0. 





K.SO 



SOLUBXLITY OF POT A8S ,UM CHtOR I8 , , Al)llIOBa Sou,,, 

OF POTASSIUM SUUUT* AT I00 AHB Vret VIM" 



0.0 

1.56 
1.63 

2.46 



35.60 
34.64 

35.96 

28.58 



KCl 



<fc. ptr 100 fit* tat, 101. 

^-.- ra g,^.. ; ,^..,.. > y\.. ..... ....... ff 

V 80 * tci " ^ 



iS-76 



8.58 
0,0 



X'll.l 



t*. 

10 

15.8 

20 
3 



30.9 
28 

33-4 
34-7^ 
36.1 



r. 
40 



Observw. 

1.32 (Prechfc ft Wit,) 
2 . J (Kopp.) 

1-43 OP- and W,) 5^ 

34.76 2.93 (VwtHbffftMwrhoffw.) 80 
I -.57 OP.wdW.) I00 



Cnw. ptr too Cms. H t C>, 

"" 



38.7 

4^-3 
43*$ 

49-2 



, 

Obsewr - 



1.68 

1.82 
1.Q4 

2,21 



ri mwi de B&at, 



?6i KALIUM K 

EQUILIBRIUM IN THB SYSTKM POTASSIUM CHLORIDE, POTASSIUM 

SULPATB AND POTASSIUM CARBONATE IN WATER. 

(Teeple, igj*).) 

Solld ftes. per 109^ gns. H g O Solid 

23' Phase ' KCl K^Scfj K^CO^ A Pliaae 

Results at 35 Results at 50 (con.) 

39.0 KC1 3 .6 121.3 K.CO i|H 

K ?i S0 4 trace 121.2 n * + K*SO 



iis.i K CO .iill 3 .6 " 121.2 " + " * KC 
38.4 1.7 - KCl * K' SO. 

3.1 114.1 " * K-COj.iiH Results at 75 

trace 112.5 ^CO^iingCr + K ? a 49.7 KCl 
2.9 " 112.7 '" * "+KC1 20.6 K^SO 

136.4 K CO . iAH 

Results at 50 48,5 1.9 K'Cl + 1C SO 

M3-1 KCl trace 135.8 " * K p 

- 17.1 K ? S0 4 5.2 " 133.5 " * " + KCl 

~ 121.2 KO.i4H 

42.2 1.8 K'vSO, KCl 



Data for the following four or more component Systems containing KCl, 
in Water, are given by Teeple, 1929. 

KCl + NaCl r Na p S0 4 4 K.SO, at 3 5, 50 and 75. 
KCl * NaCl - Na.00, 4 rcO, at 35, 50 and 75. 
KCl ^ NaCl i- Na^SO* K^SO ^ Na C0 f K p CO, at 20, 35, 50, 75 
and 100 ' * 

KCl * NaCl * Na a B 4 * K^B 4 at 35. 
KCl + NaCl * Na.B^O - 'K. B_0_ at 35. 



SOLUBILITY DATA FOR THE RECIPROCAL SALT PAIRS KCl +Na2SO4^K 2 S0 4 + NaCl. 

(Meyerhoffer and Saunders, 1899.) 
j nt Mob. per tooo Mols. H0. 

tfot Solid Phase. 







Sat. Sol. 


S0 4 . 


K,. 


Na.. 


C1 2 . 


4 


4* 




5.42 


14.39 


51. 


83 


60.8 


o 


,2 




3-35 


12.78 


50. 


93 


60.36 


o 


4 




3-59 


16.38 


40, 


75 


53.54 


16 






4.72 


17.58 


50. 


56 


63.42 


24 


.8 


I . 2484 


4-37 


20.02 


48, 


36 


64.01 


16 


3* 




16.29 


9.l6 


6x, 


,06 


53-93 


24 


-5 


1.2625 


H-45 


9-90 


58, 


46 


53-91 


o 


3 




2-75 


25.77 


17, 


93 


40-95 


25 




I . 2034 


2.94 


36.20 


14 


.80 


48.06 


17 


< 


1.2470 


I3-84 





62 


54 


48.70 


30 


.1* 


1 . 289 


50.41 


10. 08 


40 


33 


o 














* 


tr. pt. 



N%S0 4 .ioH a 04-KCI+NaCl 
N%S0 4 .roH 2 Q+Ka+K 8 Na(S0 4 ) 8 



Curves are given in the original paper and a complete discussion of the older work. 



K KALIUM 762 

SOLUBILITY OF MIXTURES OF SODIUM SULFATE, POTASSIUM CHLORIDE, 

POTASSIUM SULFATE, ETC., IN WATER, 

(Meyer holler ami Saumicn, i8yy.) 



Cl 



t" 




Solutions. 


8 




i 


Ca 


N 


aa 


a 


~ \ 


*4. 


4 


. . . 


5- 


42 


14. 


30 


5 1 - 


3 


60, 


8 8 


0. 


2 




3- 


35 


12. 


,78 


5- 


03 


60, 


36 


- o. 


4 




3- 


59 


16. 


38 


40, 


75 


S3- 


54 


16. 


3 




4. 


72 


17. 


58 


50. 


c;6 


63 , 


,42 


24. 


8 


I . 2484 


4. 


37 


2O. 


CO 


48, 


36 


64. 


,01 


*i6. 


3 




16. 


29 


0- 


16 


6r. 


06 


S3- 


'03 


24. 


5 


I . 2625 


14. 


45 


0-00 


58. 


46 


S3- 


.91 


0. 


3 


. . . 


2. 


75 


25, 


77 


17. 


03 


40, 


05 


25- 





1.2034 


2, 


94 


36. 


20 


14. 


80 


48. 


06 


*I 7 . 


9 


1 . 2474 


13. 


84 


o.o 


62. 


57 


48. 


70 


* 3 o. 


i 


1.2890 


s- 


41 


10. 


08 


46. 


33 


0, 


o 


21. 


4 












46. 


61 


4 6. 


36 


23. 


7 






. 


10. 


5* 


39- 


58 


50. 


09 


10. 


9 




I. 


45 


30. 


68 






29. 


23 


~~ 3 






16. 


25 


IO. 


03 


6. 


21 






- 3 




. . . 


x6. 


24 


10. 


03 


6, 


21 


. , 





-14 




. * . 


i. 


39 


25. 


59 


8. 


78 


32. 


94 


-14 




... 


i. 


39 


25, 


59 


8, 


78 


32- 


94 


-23. 


3 


... 


0. 


41 


15- 


*S 


44. 


2O 


58, 


97 



KN T a(SC ) 



NaCl . iHiC >-f Na 3 SO 4 , toHtO 



EQUILIBRIUM IN THK SYSIT.M POTAHAUJM (hn.ontnF, POTASMX'M SULFATE, 

SODIUM CHLOKIDK, SODIUM SUI.FATK AMI* WATKH AT Ihrrtay'NT TI-'.MPKRATURES: 

I UlnncUUs IUI8.) 

Saturation was secured by constant atirriitg at coitntunt trinparature, 

Kesutts at 11". 

(JriiN, per UK) gu)K. Il;(), 
KCI, K t $0 4 . NnCl. No.SO,. 



./of 
t. NOl. 



Sftlitl 



.088 - ri.oa 

.187 36.C/J 

'99 

a8-x - 9.81 

i 49 - i 3.?4 

.190 36.63 i.53 



KCI 



0.69 



-f-KCI 



'43 - - 18.82 ui.58 Na|SO|,roH.|< 
*7'$ " 7-3'>. 14.28 2%. 18 " 

-w>o 29.88 2.73 6.78 . Kl., . ,.., , 

.250 iC.37 - -17.96 '\.*>\ -f-.\aCI -. 

^6 - 11.04 34.90 a. 25 Nit t SO v ^- -r 
Exactly similar results are also given for o, 5o, 7 r i ami ICK>. 

Fusion-point data for mixtures composed of the various combiaations, 
KCI, K f 80 4 , UCl, Li^SO , NaCl and Na^SO., are given by Dombrowskaja 
and Klatchko, 1933. 



763 KALiUM 



POTASSIUM CHLORIDE 



Equilibrium in the Reciprocal Salt Pair 

in Water Alone and in Water Saturated with Ammonia at Atmospheric 
Pressure. (Hill ana Louclcs, 1337.) 

Results for the 3 component Systems in Water at 25 

nms. per 100 gpia. sac, solution Solid 

'(NH 4 ) ? 80 4 KCT K p S0 4 NH 4 CH Phase 

26.42 ~ KCl 

25.90 1.05 f " + K 2 S0 4 
-* o.o 10.80 " K SO 

10.36 9.59 (0.953 KjS0 4 + 0.047 (NH 4 ) ? $0 4 ) 

15.40 8.72 (0.925 '" + 0.075 " ) 

28.3! 6.12 (0.773 " *" 0.227 " ) 

39.20 2.86 (0.195 " * 0.805 " ) 

43. <i a - - - <NH 4 ),S0 4 

26.12 - ~ 16.35 " + NH Cl 

11.02 21.97 (0.166 NH^Cl + 0.834 KCl) + 

(0.975 NH^Cl * 0.025 KCl) 

26.42 KCl 

C 1 



Ona. per 100 gas. jaau solution Solid 

Phase 

KCl 



_ 


KCl 

15.26 
15.30 
0.0 


trace 

0.20 






2.85 - - - 

7.56 0.23 

11.35 

11.98 

13.54 0.20 
14.97 

17.55 " 0.07 ~" 
18.4 

4.66 ~ 33-72 

35.59 

2.86 33-59 

The results in parentheses show the composition of the solid solu- 
tions present as solid phases. 

The authors also give results for the 4 component systems saturated 
with solid phases composed of mixtures of the three solid solutions 
of the salts. They also investigated, for the purpose of industrial 
preparation of K ? 80 4 , the field in which this salt separates in order 
to learn what percentage of (NH 4 ) a S0 4 accompanies it as a contamination. 



K^SO 




(0.932 K S0 4 + 


0.068 (N'H 4 ) ? S0 4 ) 


(0.776 " * 


0.224 " ^ 


(0.676 " * 


0.324 " ) 


(0.525 " + 


0.475 " 


(0.3^2 " + 


0.658 " ) 


(0.186 " * 


0.8l4 " ) 


(0.083 " + 


0.917 " ) 


(NH ) S0 4 




" * NH 4 C1 




NH 4 C1 




(0.158 NH^Cl * 


0.842 KCl) -f 


(0.977 NH^Cl 


+ 0.023 KCl) 



1 



K KAUUM 764 

SOLUBILITY OF POTASSIUM CHLORIR IN AQUEOUS SOLUTIONS 

or MAGNESIUM CHLORIDE AT o AKD VICE VERSA. 

rrgtlsrud, iuia Tiuwpson, ww.) 



Cl 



Ows. per 100 m&. sat. aoi. Solid OM. ptr 100 JJM. m. oi. 

- ^ ^ putat /"""'"'Hgpi.. "kci" * '"^ 



o.o 21.87 KCl 26,79 2.13 KCl 4 i.u6 

5.88 15.21 H a ?- ^ *- 6 ^ i-i-6 

9.^9 11.70 " 29.70 0,49 M 

16.33 6.31 " m-68 O,oa6 M * MgCl t ,f 

25.24 2.35 M 3^^3 o.o MgCl^.titLO 



1.1.6 KCl.MgCl,.6H t O 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS MAGNESIUM 
CHLOEIDE SOLUTIONS, 

(Precht and Wittfrn Her. 314* 1667* *t,> 

Grams KCl per too Gram S*r. Sotttthm irr 



Mgtl- MfCl?, Mrf'lj. ^-----^llLi^^ 



10 


14-3 


9-9 


5-3 


1.9 


4,3 KCl 


S-7NaC 


20 


15.9 


11.3 


6.5 


2.6 


6.0 " 


*5-Q " 


30 


17-S 


12.7 


7.6 


3-4 


6,9 


'f6.o 4< 


40 


19.0 


14.2 


8.8 


4.2 


7-9 " 


46.r " 


So 


20.5 


15,6 


xo.o 


5,0 


8.9 " 


f6. 3 " 


60 


21 .9 


17,0 


ii. a 


S -^ 


9-9 *' 


t'6-4 '* 


80 


24.5 


19,5 


X3 -6 


7-3 


10.9 ** 


46,6 " 


90 


25 .8 


20.8 


14.7 


8,1 


11,9 " 


+ 6.7 " 


100 


27.1 


22 ,1 


15 .9 


8.9 


13.0 4| 


4-6,9 ll 



More recent data on the solubility of potassium chloride in aqueous solutions 
of magnesium chloride are given by Fcit and Prxibylla (1909). 

* "" OP POTASSIUM CHLOID IH AQOIOUS Soit?Tions 

or H^GKSsifiM CHLORIDE AT ioo 

Hi teili, it 34.) 



o.o 36.0 KCl 24.80 ^.60 KCl 

4.35 29*80 fl 39.89 5. is w * 1.1.6 

9.93 23.59 w tto.o i88 1.1.6 

i^-3S 17-50 w 40o 1.64 ** 

20. is 13.45 * i.o 0.71 " + MgCl f .6H/> 

1.1.6 = KCl.MgCl a .6H E (CarnalliieK 

Results for the four cofliponeat system KCl * K f SO f HgCl f * HgS0 4 

at 100 are also given by Campbell, Downes *nd $amt t 1934. 1 



765 



KALIUM K 



EQUILIBRIUM IN THE SYSTEM MAGNESIUM CHLORIDE, POTASSIUM CHLORIDE 
AND WATER AT DIFFERENT TEMPERATURES. (Keitel, 1923.) 



Gms. per 100 gms. sat. sol. 


Gms. 


per 100 gnus. { 


;at.sol. 




t. MffCl a . KCl. 


Solid Phase. 


t". 


MffCl a . 


KCl. 


Solid Phase. 


i5 


... 35. 


IO 


o. 


o 


Bischofite 


55... 


i5 


.14 


14 


79 


KCl 


i-5 


... 27. 


59 


2. 


76 K Cl + Carnalllte 


55... 


7 


.24 


23 


.40 





i5 


... 23. 


83 


5. 


49 


KCl 


83... 


39 


.80 





.0 


Bischofite 


ID 


.... 16. 


5 7 


10. 


73 





83... 


37 


.80 


I 


.01 


M + Carnal Ut(- 


i5 


7- 


66 


17. 


66 





83... 


36 


.99 


2 


.52 


Carnal lite 


25 


... 35. 


60 


o. 





Bischofile 


83... 


29.45 


5 


.80 


-4-KCI 


25 


. .. 35. 


U 


o. 


5 


-f- Carnalllte 


83... 


20 


.53 


12 


.75 


KCl 


25 


. .. 27. 


70 


3. 


70 


KCl 


83... 


i4 


.63 


18 


.3i 





25 


... 26. 


81 


4. 


56 


KCl 


83... 


14 


77 


18 


.27 





25 


... 24. 


58 


5. 


22 





83... 


7 


.15 


26 


.85 





25 


... 23. 


10 


6. 


06 





io5. . . 


43 


47 


o 


.0 


Bischofite 


25 


... 16. 


4o 


10. 


36 





io5. . . 


4o 


. 7 5 


i 


.07 


+CarnallUe 


25 


. . . i5. 


64 


1 1 . 


54 





io5. . . 


36 


.5i 


3 


.62 


Carnal lite 


25 


... 7- 


68 


'9- 


5o 





io5. . . 


3o 


.82 


7 


.00 


H-KC1 


55 


... 3 7 . 


55 


0. 


o 


Bischofite 


io5. . . 


21 


44 


14 


.83 


KCl 


55 


... 3 7 . 


38 


o. 


21 





io5. . . 


i4 


.08 


21 


.72 





55 


... 36'. 88 


0.6* 


4-CarnallHo 


io5. . . 


i3 


97 


21 


,87 





55 


... 28.74 


4- 


43 


KCl 


io5. . . 


6 


.52 


29 


.90 





55 


... 22.72 


9- 


79 


KCl 


io5. . . 





.0 


36 


.$5 





Bischofite MgCL, 


.GH a O; 


Ciirnallito 


MgCl a .KCl. 


6H S 


,0. 








The following determinations at a5 are reported by Lee and Egerton, 1928. 






Gms 


. per 


lOOgms. 


Gms. par 1 00 gins. 


f / i4 


of sat. sol. 


sal. sol. 


/ s8 of al. sol. ^ . 


sal. sol. 







Met 


;i s . 


KCl. 


Solid Phase. 


9ft 




Mg( 


^T^ 


KCl. 


Solid IMiasr. 




1.341 


35. 


54 


0.0 


MgCl s .(ilI,0 


- 




26. 


79 


3.20 


KCl | Cj.niatlllc 







35. 


14 


o.53 


4-Carnntllte 


26. 


66 


3.19 







_ 


35. 


i3 


o.38 


)> 


1.234 




19. 


83 


7.90 


KCl 




- 


35. 


47 


0.52 


w 


I . 20 1 




12. 


1 1 


13.56 







- 


26. 


81 


3,33 


KCl 


i.i8->. 




O. 


o 


26.74 


> 



K KALIUM 



766 



POTASSIUM CHLORIDE 



Cl 



IN THE SYSTEM POTASSIUM CHLORIDE, HAffHXSXflM 

AND WATRR AT TBMPKRATnxBS: AHOVE 100. 

103?*) 



d.or 


Ctea. per tOgO 


*M.JIpO 


Solid d.of CMft, p* r t 


yOjf*' H0 BollQ 


iat. sol. 


1 1^17^ 


"* cx """* 


WMMM 9*1. awl. ^"""^MtirTJ 


... ^^p*.^ ^^^ 




Results at 


100 


Resu Its 


M ISO 





100 


415 


KCl - 100 


SSH KCl 





300 


220 


11 100 


1*17 M 





$00 


108 


It ,, ^ Q -fc~ 


JI14 w 





700 


10 


" 900 


105 M 


1.307 


$07 


103 


11 + 1.1.6 1.181 864 


90 rt * 1,1.6 


1.384 


723 


9 I. 1. 


6'* > HgCl ,i|lLO 1,435 3UK4 


37 M.6*MgCLqiy) 








*'4$5 n>8 


46(167) KCl * 




Results at 


12$* 




HgCl ,i|H D 








Results 


At 300 * ^ f 





100 


480 


KCl 







300 


280 


rt 100 


687 KCl 





500 


l6o 


H _. ^ 


454 w 





700 


82 


M 500 


a<)4 M 


1-335 


690 


100 


H + i.i.6 -- 900 


163 


1.430 


890 


28 1.1, 


6f MgCl p .iiH t Ch.*j7a 1290 


SM H *MgCl. 



1.1.6 = KCl. MgClj. 6^0 (Carnal lite I 

The authors also give results for the systw KCl * NaCl * HgCl f * K ? 
at 100-200. 

Data for the System KCl * HgCl f * Nad * Mg$0 4 at ao-aoo * are given 
by Froehlich, 1929. 

Data for the reciprocal Salt pairs (KGU^ * MgBr^ ^- : -> tKBrl t t MgCl ? , 
At 20 recalculated from the results of Boeke, 1908* ^rc given by 
J'anecke, 1938. 

Data for the System KCl * RbCl * MgCl ? t H f O At a$ 4 reralcuUted from 
the results of D'Ans and Bush, 1937, are nlven by Jknecke, 1937, 1938. 



76? KALIUM 

SOLUBILITY OP MIXTURES OF POTASSIUM CHLORIDE AND AMMONIUM 
CHLORIDE IN WATER AT 25. 

(Fock Z. Kryst. Min. 28, 353. '07.) 



Grams per Liter 
Solution. 


Mol. per cent or,* 
in Solution. p. Gr. of 


Mol. per cent in 
Solid Phase. 


'NH 4 C1 


KCl. 


NBUCl. 


KCl. " 


tfH^Cl 


KCl 


o.oo 


3 rl -3 


0.00 


IOO-O 


.1807 


0.0 


100 


22. 8l 


293-3 


9-41 


90-59 


.1716 


I .21 


98.79 


35-39 


278.7 


15.04 


84-96 


.1678 


2 .11 


97.89 


89.17 


273.2 


34.26 


65-74 


1591 


6.18 


93.82 


127.8 


234.6 


46-59 


53-44 


I 493 


8.90 


91 .TO 


147.2 


204.2 


5 1 6 3 


48.37 


.1461 


io-53 


89.47 


197-3 


157-7 


63.56 


36.44 1.1391 


17 .86 


82 .14 


232.5 


116.8 


73-49 


26.51 1.1326 


60.20 


39-80 


244-5 


123.0 


73 48 


26.52 1*1329 


76.88 


23.12 


261.9 


III.O 


79.10 


20.90 1-1245 


97-51 


2.49 


259.0 


IO2.2 


82.14 


17.86 I.I2I2 


97-79 


2.21 


278.6 


53-16 


87.96 


12.04 I.I009 


98.85 


I.IS 


320.7 


31.24 


93-45 


6.55 I.09I2 


99-33 


0.67 


273-5 


o.oo 


100 -OO 


o-oo 1-0768 


100 -0 


o.oo 



The following additional data for the above system are given by Biltz and 
Marcus (1911). The results show that NH 4 C1 + KCl form a series of mix- 
crystals broken by a gap which extends between about 20 and 98 mol. per cent 
NHiCl in the crystals. 



Composition of Sat. Solution. 



Composition of Solid Phase. 



Gms. per 
Sat. 


TOO Gms. 
Sol. 


Mols. per 1000 Mols. 
H,O. 


Gms. per 100 Gms. jtf o] % 
Crystals. NH<C1 in 


)NH 4 C1. 


KCl. 


NHiCl. 


KG.' 


NH 4 C1. 


KCl. ^ 


Crystals. 


5-13 


22.29 


2 3 .8 


74.2 


I. 21 


98.79 


i-7 


7 


2O.4O 


32.5 


67.9 


2.22 


97.78 


3"* 


II 


18.04 


52 .2 


61.4 


4 


96 


5-5 


13-73 


l6.II 


65.9 


55-5 


5.89 


94-11 


8 


15.46 


14-53 


74-4 


50.2 


7.24 


92.76 


9.8 


19-54 


T2.l6 


96.3 


43 


II .20 


88.80 


14.9 


22.O4 


10.49 


109 


37-4 


16.90 


83.10 


22.1 


21.68 


IO.4O 


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 carnellite and 
potassium chloride carnellite 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). 



KALIUM 

EQCnUBRltIM IH THE SYSTEM POTASSIUM CttLOftZDI, AMMONIUM 

CKLORX&I AM WATM. 
(J Intent, lif^a 

The J&necke method of expressing th* concentration of the saturated 
solution is in terms of the number of Cm. Hols. H f C) required to dis- 
solve too gro. mols, salt or salt mixture of tftr determined wilecular 
composition. 

In the present case the salts lorn mixed crystals and the imlui phases 
in contact with the solutions Ar* couponed of such mixed crystals con- 
taining varying percentages of the two salts. 



of dlMOlwtf fts*. mi* H ;> a to 

la P. a&l Cltaolvt tOO *** 

""""^""""TnTcr" 11 '^ aou. *it nit curt 



100 0.0 

80 20 

60 40 

40 60 

28.5 71.5 

30 SO 

100 

100 0,0 

80 30 

60 40 

40 60 

37.5 73*5 

20 80 

100 



100 0,0 

80 ao 

60 40 

40 60 

26 74 

20 80 

100 

100 o.O 

80 ao 

60 /|t> 

40 60 

24 76 

20 80 

100 



*00 0,0 

ao Bo 

100 
100 

IS- 5 84 
o 100 

<i) These values by Askew any 'and 
-'-e also gives siwil4r 
the reciprocal 



It} 30 


100 Mol, 


. KCl 




ITW 


91 w 


Ul 




130O 


90 


ID 




1030 


84 


(l! 




950 


Hi 


* * 95% Hol. 


ft NILQ 


9^0 


96.5 




" lit 


1000 


100 




H 


Results AI m ( 


Q 






1310 


too Mol, 


, % KCl 




1090 


? 


* 




Buo 


? 


M 




?l|0 


75 


w * s Hot % 


NH.Cl 


730 


? Mol* 


$ NH 4 tt 


4 


800 


tetit 


i 




Results 41 no* 


> 






1010 


100 Mol, 


% KCl 




6 ? 'o 


66 


#* 
11 93,5 Mot, 


ft NH.Cl 


6 30 


? Mol. 


ft WLCf 


4 


650 


100 






Results At 60 








90$ 


100 Mol. 


% KCl 




760 


? 


M' 




650 


? 


ft 




$50 


? 


W 




S**> 


in 


w +,9i Mol, I 


NH.Cl 


530 


? Mol. 


f MHaCl 


4 


sno 


100 


* 




Results AI 80 








810 


loo Mol. 


I KCl 




30 


38 


w * 90 Hol. i 


K NH.Cl 


1150 
Results At 100 


100 Hol, 

.0 


$ fH 4 Cl 


% 


730 


ioo Hol. 


S KCl 




160 


38 


M * ^i Mol. % 


r<ti L>4 


390 


100 |kf | ^ 


1 NILC1 




my and Ntsl 


f^ 19^00 


* 4 




if results for 

.1 pair KCl * N 


e^ttiiibriBA in the system cm- 

H KO NH j:i t KH0,.;Aitoasy 


IttltS for th* a 


I* .* L*ft * 


t-- *^f K <r i 


y | 



769 KALIUM 

SOLUBILITY OF POTASSIUM CHLORIDB IN AQUBOUS SOLUTIONS OF AMMONIA. 

(Ouyer. Dleler and Schmld, 1934.) 

The authors present their results in the form of a diagram but do 
not give their experimental determinations. The following approximate 
values were estimated from the published diagram. 



K 



Results at -15 

OB\a. per 100 g%3. aat. sol. 



Results at + 25 



Solid 
Phase 



KCl 

55 4.0 

60 3-1 

70 1.7 

80 0.8 

90 0.35 

100 0.2 

SOLUBILITY OF POTASSIUM CHLORIDE IN LIQUID AMMONIA 
DETERMINED BY THE SYNTHETIC METHOD. 

(Pacschetce and Tanne, 1935.) 



0ms. per 100 gps. 


sat. sol. 


' NH 3 


KCl ^ 


62 


4-0 


70 


2.4 


80 


1-3 


90 


O.S 


100 


0.1 



Solid 
Phase 

KCl 



-76.6 
-76.6 

-76.7 
-76.8 
-76.9 
-77.0 
-77.2 
-57.9 
-q.5.0 
-35.2 



Gtos. KC1 par 
100 ^a. at. sol. 



0.078 
0.115 

0.167 
0.193 
0.209 
0.219 
0.252 
0.219 
0.209 
0.193 



Solid 
Phas 



NH 



NH 
KCl 



+ KCl 



-33.9 
-19^4 

~ 0.6 
- 

+15-0 
25 

18.9 
31.2 
44.2 



Oms. KC1 per 
100 *. sat. sol. 

0.213(1) 
0.167 

o.ui 

0.132(2) 

0.115 

0.04 (3) 

0.102 

0.089 

0.078 



Solid 



.The authors al.so give results showing that the solubility of KCl in 
liquid ammonia is increased to almost double by the presence of NaCl 
or of Nil Cl. 

(i) Jonnson and Krumboltz, 1933; (2) Linhard and Stephan, 1933~193<; 
(3) Hunt, 1932. 



p - 



THE SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF MIXTURES 

OF OTHER SALTS. 

The polythcrms of the four salt points of the potassium chloride field in quinary 
systems of oceanic salt deposits have been redetermined with great ear by 
Dr. Scrowy, 1928. This is a repetition and extension of the fundamental work 
of Van't Hoff, D'Ans and others. Results at temperatures between and 120 
arc given for the equilibrium solution Q (Van 1 ! Hoff) in contact with K Cl + Na Cl + 
carncllite + kainite % or kiesicrite; at temperatures between Co. 5 and iaa for 
the equilibrium solution P in contact with K Cl + Na Cl + glascrite + langbeinito ; * 
between o and 110 for the equilibrium solution F in contact with K Cl 4* Na Cl ~K 
glascrite; between o and 12,0 for the equilibrium solution K in contact with 
K Cl + Na Cl ^r carnellite and between 23 and 120 for the equilibrium solution K 
in contact with Na Cl + kainite + kiesierite + carnallite and with K Cl + Na Cl + 
kicsierite + langbeinite. For additional references see also magnesium chloride, 



K 



KALIUM 

POTASSIUM CHLORIDE 



770 



Cl 



SOLUBILITY OF POTASSIUM CHLORIDB rn AQUIOOS SOLUTIONS OF 
SODIUM CHLORIDE AND Viet VERSA* 
(Cerate n$ 



U.of 
c. aol. 



. pur 100 

kcT """""""" 



-22.9 





5,81 


20. 17 


-21.8 





2.60 


21.71 


-21.1 


, 


, 


21.07 


-17.8 





9*01 


14.40 


-13- 7 





13-64 


7-59 


-iq.7 





19*5* 





-11.9 





6.49 


21*41 


-10.0 








24-70 


-2,3 





6,96 


32, 54 


* o.i 


~~ 





26.27 





1.154 


21.92 


0.0 


M 


1*175 


16.09 


7.67 


It 


1,300 


in. 39 


14.83 


n 


1.221 


8.46 


20,03 


n 


l.34 


7.a8 


23.40 


n 


1.226 


5.10 


23-5* 


it 


1.218 


2*58 


34.86 


n 


1.209 


0.0 


36.25 


10 


1.233 


8.71 


21.66 


20 


1,174 


a5- 57 


0.0 


H 


1.190 


19-48 


7.36 


II 


1.210 


14.89 




M 


1.221 


12*34 


.17.64 


It 


1,234 


10.19 


20.03 


II 


1.333 


6.98 


32.65 


tt 


1.213 


3.54 


24.47 


M 


1.201 


0,0 


36.34 


30 


1.235 


11,70 


30, 3$ 


40 


1.189 


28,65 


0.0 


H 


1*201 


33*44 


7.19 


II 


1.218 


17.05 


14.04 


II 


1.236 


13.16 


19.66 


W 


1.231 


8.94 


31,87 


If 


1.207 




34.15 


n 


1.192 


0,0 


36.64 


50 


1*237 


14.70 


19*03 


60 


1.199 


11.29 


0.0 





1.210 


15-1*1 


6-90 


n 


1.224 


19.79 


13.53 


n 


1.238 


l6. 07 


18-S7 





1.220 


10,97 


21.17 


n 


1.202 


5-71 


35.94 


n 


1.184 


0.0 


27.03 


70 


1.239 


17.59 


18,05 


80 


1.205 


33-59 


0.0 


" 


1.216 


37,59 


6,79 


V 


1.229 


23.34 


11.17 


H 


1 . 24 1 


19.03 


17.59 


tt 


1*223 


14.10 


20.01 


H 


1.199 


7.38 


31-53 


It 


1.17S 


0.0 


37*$* 



KCi 



KCl 
NCl,aH t O 

KCl 



NaCl.aH f O 

KCl 



KCl 



N*Ci 



KCl * NuCl 



Had 



KCl * NaCl 



JCC1 * HaCl 



KaCl 



KCl * HiCi 



HaCl 



HaCl 



771 



KALIUM K 



POTASSIUM CHLORIDE 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 
SODIUM CHLORIDE AND VICE VERSA. (Con.) 

(Cornec and Kronbach, 1932.) 



90 
100 



108.5 
111.9 
108.7 



d. of 
a at. sol. 

1.242 
1.209 
1.219 
1.232 
1.244 
1.232 
1.20O 
1.166 
1.245 



1.209 
1.246 
1. l62 



One, per 100 gna. ec. eol. 



KC1 


WaCl * 


20.32 


17.24 


35.69 


0.0 


29.95 


6.48 


24.88 


12.69 


21.68 


16.90 


19. 12 


18.12 


10.25 


22.57 


0.0 


28. OQ 


23.04 


16.58 



Solid 
Phaae 



KC1 NaCl 



NaCl 



NaCl 



KC1 f NaCl 



Results for the b. pts. 



36.50 

23.28 

o.o 



o.o 
16.52 
28.30 



KC1 

" + 
NaCl 



NaCl 



The above determinations for the solutions simultaneously saturated 
with KC1 + NaCl are in good agreement with the values reported by 
Blasdale, 1918, but not with those of the earlier workers including 
Precht & Wittgen, 1881; Etard, 1897; Leather and Mukerje, 1913; 
Reinders, 1915; and D'Ans, 1915. The more recent determinations of 
the system at 20 by Di Capua and Scalletti, 19271 are in satisfactory 
agreement with the above results. 



Cl 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 
SODIUM CHLORIDE AND VICE VERSA AT TEMPERATURES ABOVE THE BOILING POINTS. 

(Cornec and Krombach, 193?.) 

The determinations were made in a small inoxydizable steel autoclave 
in which Jena glass recepticles were fitted in such a manner that the 
solution after saturation in one by gentle agitation could be filtered 
into the other by inverting the autoclave. 



t 


Gas. per 100 
0*8. aat. aol. 

. IV . n L. . 


Solid 
Phaae 


t o 


tea 
gna. 


. per 100 
aat. aol. 


Solid 
Phaae 


'KC1 


NaCl 


J KC1 




NaCl 






120 


37. 


65 


0. 





KC1 


140 


19- 


07 


19. 


6l 


NaCl 


rt 


32. 


28 


6. 


24 


n 


n 


9- 


98 


24. 


13 





n 


27. 


33 


12. 


25 


tt 


" 


0. 





29. 


30 





n 


24. 


23 


16. 


35 


"+NaCl 


149 


27. 


44 


l6. 


08 


" +KC1 


rt 


17. 


29 


19- 


69 


NaCl 


169.5 


42. 


42 


0. 





KC1 


n 


9. 


48 


23. 


66 


" 


ti 


37. 


24 


5- 


92 


n 


it 


0. 





28. 


60 


n 


" 


33. 


04 


11. 


41 


tt 


130 


25- 


29 


16. 


33 


" + KC1 


rr 


30. 


72 


14. 


52 


M 


140 


39- 


60 


0. 





KC1 


it 


29. 


63 


16. 


03 


" +NaCl 


n 


34. 


43 


6. 


17 


ii 


ti 


23- 


38 


18. 


78 


NaCl 


ti 


29. 


71 


11. 


86 


rt 


" 


15. 


24 


22. 


66 


M 


it 


26. 


45 


16. 


17 


"+NaCl 


tt 













Ota a. per 100 
H>aa. sac, aol. 
IccI ' X NacT 



solid 
Phaae 



169.5 8.68 25.93 NaQ 
" o.o 30.62 " 

189*644.34 o.o KC1 
" 39.36 5.68 " 
" 35.44 10.86 " 
33-38 13-64 " 
" 31.74 16.33 "*NaQ 
25.58 18.78 NaCl 
" 18.36 22.01 " 
" 9.88 26.13 M 
11 o.o 31.45 " 



K KALIUM 77^ 

POTASSIUM CHLORIDE 

SOLUBILITY OF POTASSHW CHLOXZDS IN Aqusons SOLUTIONS OF 
SODIUM CHLOKIPI AHD- Vici VI*SA AT TKMPMATHHIS Anovi 100, 





d, of 


Oas. ptr iOOj^ 


pts. 


HJ3 tolU 


fl-or a 


to*. pr 


%, 


H|P 8olU 


c 


sat, toL 


Tar" 




**"** ^ **** 


& MU Ml. ^ 


Ktfl 




A Phw 


100 


. 


480 


100 


KCl 


170 1.305 


5*13 


293 


KCliNaCl 


It 





440 


150 


H 


l8O 1.3l8 


577 


300 


M M 


n 





400 


200 


H 


1K 1 . 330 


614 


309 


n 


n 


_ 


360 


350 


M 


JOO 


741 


100 


n 


n 


1.2^5 


359 


257 


" +NACI 





70S 


*sa 


w 


it 




300 


aSo 


NaCl 


w . 


682 


300 


it 


110 


1.255 


390 


259 


KCUNaCl 





66l 


350 


M 


120 


1.264 


415 


265 


It H 


w i 3*c> 


6$^ 


319 


M -fKaCl 


130 


1.274 


440 


370 


tt M 





600 


123 


K'aCl 




1.282 


465 


275 


H 


" mom. 


500 


310 





ISO 





606 


100 


ft 


** 


400 


164 


w 


N 





570 


ISO 


H 


n 


300 


389 





' 





533 


200 


M 


aao - 


698 


332 


KCltNaCl 


N 





500 


2SO 


ft 


330 


722 


338 


H 


It 


1.289 


486 


aSo 


H *H4Cl 


350- 


7C9 


351 


n H 


K 





400 


303 


HaCl 


270 


8l? 


374 


if n 


II 


__ 


300 


333 


M 


380 ~ 


847 


|8^ 


H It 


l60 


1.295 


508 


235 


KCUNaCl 


J00 ' 


900 


40 a 


H tl 



SOLUBZLZTY OF POTASSHIN CKtOftfDI IK AdtllOtfS SOI.nTZOKS OF 

VtCI fllSA AT l.$ ft 
4 Muuuior. IfffTJ 

To standard solutions of one of ihc sails AA of the other sail 

was added and the nixturet heattct 10 6o Mitt ihen cooled Mil shaken at 
18.5, until eqtttilibriun MM atiAlned, A given folawc* of ihc SAIU rated 
solution was evaporated to dryatst 4nd fron the weight of the residue, 



the concentration of the orifii&l solvent 
the original solvent md final mttwrjiifd !yfio 
salt present in looocc, of the satttrntctl solution 
results thua obtained .agreed satisfaciorlly with 
upon chloride determinations* 



the densities of 
tht weight of tach 
c*lcl4te4, The 



Da. Hols. Nad 
per liter 
aq. solvent 

0.0 

o.a 

0^6 
i.o 

3-0 
4*66 



fiat. 
aol. ' 

1738 
175^ 
,1766 
.1793 
.1840 



1.2070 l6l.73 



ton. j':r 1000 
60. M&. ML 



o.oa 298.50 

10.26 290* so 

20.62 281.58 
31.06 373* *4 
256.74 



nwr 



ft.}, 



0.0 
0,3 
Q.it 
0.6 
1.0 
-5 
1*837 



a.r 



Mi. 



ten, I'M tODO 

. ML, ML 

ntci*" ira"" 



i.aoi? o.o 316.30 

I.J01S M4 310. iO 

1*2090 J6.S4 304*64 

I *J!94 66.72 384.50 

1.2383 100,66 368.02 

i ,2343 ian,i6 257-22 



773 KALIUM 

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. 


Cms. per 100 Gms. 
HA 


Sp. Gr. 
Sat. Sol. 


Gms. per 100 Gms 
H ? 0. 


Sp. Gr. 
Sat. Sol. 


Gms. per too Gms. 
H 2 0. 


Solid Phase 
in 
Each Case. 


KG. 


NaCl. 


KC1. 


NaCl. 


KCI. 


NaCl. 


1.176 


34.61 


O 


I 


194 


40.60 


O 


I 


222 


53.58 





KCI 


I.IQ7 


26.60 


10.13 


I 


207 


31.42 


10.68 


I 


236 


45.01 


10.66 


" 


.213 


19.65 


20.61 


I 


235 


24.43 


20.99 


1.262 


35^4 


22.87 


" 


237 


14.92 


30-36 


I 


248 


18.23 


30.60 


I 


262 


33-12 


28.12 


" 


.240 


15.36 


29.61 


I 


242 


18.74 


30.32 


I 


264 


32-45 


28.26 


" 4-NaCl 


.233 


14.76 


30.38 


I 


247 


19.13 


29.Q2 


I 


235 


27.15 


29.18 


NaCl 


.224 


9.70 


32.40 


I 


222 


10.49 


32.50 


I 


223 


13 


33-93 





I-I93 


O 


35.63 


I 


107 


O 


36.53 


T 


1 80 


O 


38.72 


u 



Results are also given for 30. 

For results in the systems Potassium Chloride, Lead Chloride and 
Water see under PbCl g 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 
RUBIDIUM CHLORIDE AT 25. 

(D'Ans and Bush, 1937.) 

C] 

Oka. Mols. per Solid Phase Ota. Hols, per Solid Phaat 

1000 ga.^Mols. H 2 Mixed crystals loop gn.^Mols. H g O Mixed crystals 

' Rb Cl e K_ci_ x containing 'm <n K ClI N containing: 

C f, C. f, K K, Id <f> 

o 43.5 100 Mol. % K 2 C1 2 iu;a 22.5 67.3 Mol. % K Cl g 

10.0 37.6 97.6 " " 51.0 17.5 41.8 " " 

19.2 33.5 92.6 " " 59.3 10.4 i$.S " " 

31.0 28.0 8/1.5 " " 70.1 0.0 " " 

Results are also given for the guarternary System KCI + RbCl + MgCl 
at 25. * 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF STANNOUS 
CHLORIDE AT 25 AND VICE VERSA. (Fujimura, 1914.; 

Gms. per iop Gms. H0. Gms. per 100 Gms. H 2 0. 
SBC KCT Sohd Phase. ^g- , Solid Pha, 

O 34-73 KC1 58.48 17.85 Sna a .KCl.H 2 

2.86 32.17 " 81.78 19.06 

4-37 34.o8 107.65 17.79 

5-95 3I-76 SnCls-aKCLaHaO 170.70 21.26 

5- 8 3 3^S " 247-5 24.38 

10.24 27.30 337-26 25.51 

17.42 24.68 " 290.30 19.66 SnCla.2H a O 

27.88 24.40 " 235.50 7.49 

34.28 5.99 222.5 2.73 

54.19 19-45 SnQ a .KaH s O 234.05 



K 



Cl 



KALIUM 

SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE AQUEOUS SOLUTIONS OF 

METHYL ALCOHOL AT o ANI> AT 25. 

lArrastronf tmi Eyre* i^iO"ii.) 



Wt. % 

CHJOH 

in Solvent. 

O 
0.79 

x-57 

3-i 
8.76 



Gmi, K.CI per 10 (trw. Sat. Sol. t: 



22.06 
21-74 
21.30 

20, 6x 

17.84 



26 , 69 
26.42 
26,01 



SOLUBILITY OF POTASSIUM CKLOREDK IN AQUEOUS METHYL ALCOHOL AT 25. 

I; Mdntoih, j<jo t t-) 



Solvent. 



(Hen and Aixtav, 3 
GIM. KO 



a W 

0.9971 
0.9791 
0.948% 
0.9180 



O 

10.6 
30. B 
47.1 



JUI 

ssoi. 

1.1782 

1.12$ 

1.033 
0,9679 



per too cc. 

1*1. Sot, 



24- S3 
7^61 



rf . 


Wt, *-iT 
UW>I , 


-y- 

S*i. Sol. 


0.8830 




o,c'jo64 


0,8489 


78.1 


0.8607 


0,8167 


o8.g(?) 


0,8242 


0.7^82 


IOO 


0,71)37 



Gm. KC1 

per 100 oc. 
Stt. Sol. 

3-44 



o 75 
0-43 



100 gms. methyl alcohol dissolve* 0,53 gm. KCI at 25*. (Turwer wl 
ethyl " 44 o.oaa " " 

propyl " 4I 0.004 " " " 

amyf " 4< 0.0008 " ** 

Potassium chloride is insoluble In CHiOH it the crtt. Icrnp, 

SotnuiLXTY or PotAfttixtiM Ctoif in Aoutmii 

SoutTXona or MKTHYL ALCOHOL AT 35. 

(lK*rlof ifld Hirtiiu tt^.l 

Coeipoaltian^of fiolvau. in %. Mis. XC1 do0*iywi of Uuvmt, in 

r woo *. /nicv^^^^ra;^^*^ 



. 1910.) 



Kd 



1000 



0.0 


0000 


4*836 


19a8 


o.iiSoa 


0.6487 


11,10 


0.0656 


B.^lS 


69.74 


0.5645 


0,3766 


20.11 


0*1240 


3*830 


78.98 


0.6787 


0,2193 


29.87 


0.1933 


2*07? 


Ik*, us 


0.6983 


0.200$ 


39.93 


0*2721 


1476 


-MK^S 


o8jft8 


0.1135 


SO. 65 


0,366l 


0.9561 


100,00 


1,0000 


0.0707 



Water 



SoLOBXtiTY or POTASHXOM 
of BTHYI. AH 

(XtlU&n 
Ofc MU, Kf4,ptr Uur 

wt ^ ' *>.a ii t i 



Xt 



25.96 Wt. 


% CH OH 


1 ,700 


uSf)fi 


i afe , H 


141.4 


45.13 


* 


0.&I01 


o*ei?ao 


6^.65 


6487 


74.88 


* 


o.kftH6 


0.^1 JI 


U*o6 


15.81 


100.00 


t* 


0*ossft 


o,o*<jo 


i.i8 


4*l8 


25.07 % VI 


rt * C t H 8 0fl 


I 607 


1.751 


1x9.8 


130.9 


50.01 


ti 


0.5860 


0.60()4t 


in. 66 


44.77 


75*03 


tt 


o.iia7 


w, 124$ 


8.4 




97.3 


M 


0.00 


0,00$ a 


r 


0*39 



100 gms. aaueons 50 wt. ptrceit C H^OH Molution 6.0 I 

t 



at 20 and 15,3 gws, 



KCI 



100 



775 KALIUM 

100 gms. 40 wt. per cent alcohol dissolve 5.87 gms. KCI + 12.25 g ms - NaCl at 25. 
100 gms. 40 wt. per cent alcohol dissolve 5.29 gms. KNO; -f 10.06 gms. KCI at 25. 

(Soch, 1898.) 

TOO gms. abs. ethyl alcohol dissolve 0.034 gm. KCI at 18.5. 
100 gms. abs. methyl alcohol dissolve 0.5 gm. KCI at 18.5. 

(de Bruyn, 1892; Rohland, 1898.) 

SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE SOLUTIONS OF ETHYL 
ALCOHOL AT o AND AT 25. 

(Armstrong, Eyre, Hussey and Paddison, 1907; Armstrong and Eyre, 1910-11.) 



Wt. % 
CjHsOH 

in 
Solvent. 

O 

I.I4 

2.25 

4.41 

8.44 

12.13 

18.69 



Grns. KCI Dissolved per 100 Gms. 
Sat. Sol. at: 



0. 


25. 


22.1 


26.44 


21 .6 


25.91 


2O.9 


25.29 


19.7 


24.21 




22.46 



15-5 



17.42 



<'l* o 

Sof. Sat. 
I.I8I3 

I-I754 
1.1689 
I.I568 
I-I357 

1.0847 



SOLUBILITY OP POTASSIUM CHLORIDE IN AQUEOUS ALCOHOL AT: 



(Schiff Liebig's Ann. 118, 365, *6i.) 



14.5 

(Bodl&nder Z. phyailc. Ch. 7. 3'. '91.) 



Sp. Gr. 
of 


Wt. 


G. KCI per 


Sp. Gr, 

of Snt 


Grams per TOO cc. Solution. 


Alcohol. 


Alcohol! 


Alcohol. 


Solutions. C2fiUW. 


H 2 O. 


KCI: 


0.984 


10 


19 


.8 


1 


.1720 


, 




88 


.10 


29 


.10 


0-972 


20 


14 


7 


I 


.1542 


2 


79 


85-78 


26, 


.85 


0.958 


30 


10 


7 


I 


I 3^5 


4 


.98 




oo 


24, 


.67 


0.940 


40 


7 


7 


I 


1075 


10 


56 


79 


63 


20 




0-918 


5 


5 


.0 


I 


.1085 


15 


57 


75 


.24 


17, 


.24 


0.896 


60 


2 


.8 


I 


0545 


20 


.66 


7o 


.52 


14, 


.27 


0.848 


80 





45 


I 


0455 


24 


.25 


67 


05 


13 


.25 


Gerardin's results 


at 15 agree 


O 


9 6 95 


40 


.42 


5 


.18 


6 


35 


well with 


the above 


deter- 


O 


93*5 


48 


73 


40 


.60 


3 


.82 


minations. 


o 


.8448 


68 


63 


J 5 


55 


o 


30 



30 and 40. 

(Bathrick J. Physic. Chcra. i, 160, '06.) 



Wt. 

per cent 
Alcohol. 


Gms. KCI per 100 Gms. 
Aq. Alcohol, 


"At 30. 


At 40.' 


O 


38.9 


41.8 


5-28 


33-9 


35-9 


9-43 


30.2 


33-3 


16.9 


24.9 


27.6 


25.1 


19.2 


21.8 


34-i 


15-6 


17.2 



Wt. 


Gms. KCI per TOO Gms. 


per cent 


Aq. Alcohol. 


Alcohol, 


At 30. At 40 


43-1 


11. 1 13.1 


55-9 


6.8 8. a 


65 .9 


3-6 4-i 


78.1 


1.3 1.6 


86.2 


0.4 0.5 



K KALIUM 776 



SOLUBILITY OF POTASSIUM CHLOKIDK IN AQUEOUS ALCOHOL. 

(Genudin Ana. chim. ph>*. [4} 3* *4Q-. '65.) 

Interpolated from the original results. 

Gram* KCl per too Cmv Aq. Alcohol of Sp. Or.: 



Cl 



*. 


0-0904 

a e .e 




0.0848 


0479.1 

i\A 


I0;l 


OiOnyj o OV9 o H^fty 

** |8 - 4tf ** fto 


0^344 


wt."%. 


wt:%\ 


Wt.%. 




Wt. 


%. 


Wt %. 


Wt, 


%. 


Wt,% 


o 


23-4 




I9-S 


iS-5 


"S 


7 


.0 


4-0 


I , 


' 7 


0,0 


s 


25.0 




21 .O 


x6,a 


xa.8 


8 


.0 


4 8 


2 , 


>a 


0.0 


xo 


26.4 




22-S 


x8.o 


14.0 


0- 


-o 


C t) 


2, 


'7 


o.o 


I S 


26.8 




24.O 


19.2 


15 .2 


10 


o 


6,4 


3 


i 


0.04 


20 


29.1 




25.3 


20,3 


16,1 


10 


.8 


7 .a 


3- 


'S 


0.06 


25 


30,4 




26.8 


21 .5 


17,! 


n 


,6 


7 9 


3- 


9 


0.08 


30 


3i-7 




28.0 


22 .6 


I8,2 


11 


S 


* 5 


4, 


2 


0,10 


40 


34*3 




30.8 


24-8 


30, 


14 


o 


9,0 


4, 


,S 


O.20 




37.0 




33-5 


27.O 


21.8 


*5 


S 


10.8 


S 


,2 


Ot 3 


60 








* * * 


, * . 


16 


.8 


xi.8 


S 


S 


0.40 


SOLUBILITY 


OF 


POTASSIUM CIILOKIUK IN 


AQUROUH 


SOLUTIONS 


OF 


ETHYL 


ALCOHOL AT 


as*. 












(MvlftUiftht i : # 














Wt, % 
C a H 8 OH, 


Mob. KCl 

l*-r Liter. 


CJmi, KC! per 
loocc. St. Sol. 


t 


Ut **! 




MofeKCI 


too cc 


KG p 


O 




4. 


18 


31.18 




*6o ' 




0S^ 




4 


iis ' 


IO 




3 


21 


23.03 




70 




0.305 




2 


,27 


2O 




2. 


40 


17.89 




80 




0,125 




O 


93 


30 




X. 


7 8 


I3-37 




90 




0,042 




O 




40 




X. 


26 


9.40 




100 




o.oxx 




O 


!o8 


50 




o* 


8 4 


6.26 

















Soumrtm o? POTASSIUM Cfttomt in AQIISOITS S^tttnoHS or 
BTHYL ALCOOL AT 



Results At 25* ItaittU* At 16* , 35 And 35 

(FUtt a Jorotn, 1938.) (rtmtr t4 HtUoft, !M.) 



W't. % CgHgOH tei. KCi ptr too Wt.f*rn C^H^W few. <CC1 pr 100 P**^ #* toiijitt_ 
in aoivtnfc ipui* aolvvnt in toivwit /"""'"*a> " w "'"* "" 



0.0 


15.86 


86.11 


0. 


0.3778 


0.1134 


20.4 


19.70 


89.6 


CK I4l^ 


0* I7ifH 


0* J^9$ 


42. S 


q.i6a 


93-1 


0.^63 


,1084 


0.1207 


67.9 


2.278 




0*0431 


0*05OO 


0.0603 






100.0 


o*oa6s 




0*032$ 



777 



KALIUM ] 



SOLUBILITY OF POTASSIUM CHLORIDE IN PURE ETHYL ALCOHOL SOLUTIONS 
OF AMMONIUM NITRATE AT 25. 

(Seward and Schunb, 49%.) 



per liter solvent 

. 000 

0.000l88 

O.OO0466 

0.000992 

0.002352 



On. Hols. KC1 
per liter sat. sol. 



per liter solvent 



0.003108 <= 0.2318 gm. ) 0.00480? 

0.003125 0.008587 

0.003141 0.01947 

O.003327 0.05129 
0.003716 



0m. Mola. KC1 
per liter sat. sol. 

0.005020 
0.007229 
0.008827 
0.011131 



SOLUBILITY op POTASSIUM CHLORIDE IN SEVERAL ALCOHOLS AT 25 

(Larson and Hunt. 1939.) 



Alcohol 



ci.of 
alcohol 



d.of sat. 
solution 



Ons. KC1 dissolved 
per 100 gns. alcohol 



Methanol 

Ethanol 
i-Propanol 
i-Butanol 
2-Propanol (iso) 
2-Methyl-i-propanol 
i-Pentanol 
2-Butanol (iso) 



CllgOll 


0.7866 


0.7907 


C H 5 OH 


0.7851 


0.7852 


C1! 3 CH 2 CH 2 OH 


0.8001 


0.7994 


ai 3 (CH 2 ) 2 CII OH 


0.8057 


0.8058 


CH 3 CHOIICH 3 


0.7810 


0.7809 


(CH 3 ) 2 CHCH OH 


0.7979 


0.7980 


CH,(CH 2 ) 3 CII 2 OH 


0.8095 


0.8096 


CILCFLCHOHCH, 

32 .3 


0.8025 


0.8022 



0.5391 

0.0294 
0.0061 
0.0030 
0.0023 

0.0020 
0. 0022 
0.00084 



20 
30 
35 
40 
M-5 
50 



SOLUBILITY OF POTASSIUM CHLORIDE IN SEVERAL ALCOHOLS 
AT DIFFERENT TEMPERATURES. 

(Kirn and Dunlap, 1931.) 



On. Hols. KC1 per 100 gmamols. of: 



Methanol 


Ethanol 


Hropanol 


Iso Propanol 


Bucanoi^ 


"Tso ButanoT' 


CH 3 OH 


C 2 H 5 OH 


C^OH 


<W> H 


C 4 H 9 OH 


C 4 H Q OH 


0.833 


0. 1270 


0.00700 


0.1235 


0.00822 


o, 00326 


0.729 


0.1378 


0.00796 


o. 1300 


0.00852 


0.00356 


0.691 


0.1443 


0.00793 


o. 13110 








0.642 


0. 1454 


0.00773 


o. 1390 


0.00904 


0.00400 


0.528 


0.1277 


0.00683 


0.1295 








0.415 


0.0845 


0.00473 


o. 1060 


0.00925 


0.00407 



Cl 



SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE AQUEOUS SOLUTIONS OF 
PROPYL ALCOHOL AT o AND AT 25. 

(Armstrong and Eyre, 1910-11.) 



Wt. % 
fc GjH 7 OH 
in Solvent. 

I 

1.48 

2.91 

5-66 



Cms. KC1 per 100 Cms. Sat. Sol. at: 



22.o6 
21.25 
20.49 
18.97 



26.44 
25.94 

2S-23 
23.82 



K KAL1UM 778 

POTASSIUM CHLORIDK 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF 

I so PROHYL ALCOHOL AT 35 

. *nu Chtn ifTM.l 



The results locate the bi nodal carve of the systems .ind include A tie 
line * which shows the composition of two layers in contact with each 
other and the plait paint, PP, at which the two liquid layers become 
homogenous. 

Ohm. pr tOOjpjl^ wt. oiuilon 1 5LJSl^J2Jt mt * 
^___~-..- __-;__->, / ^^-^ r 1 ,,. 

13.72 17- 8* l6. Hi 9.17 

17.64 15.1? :7.s H.*:i PP 

22.8? 13.95 43.'*6 7. An 

29,34 11.04 51-I1 5-ia 

SOLUBILITY or POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS or 

I so PROPYL ALCOHOL AT DIFFERENT TEMPERATURES. 

(fmtr MU) Wiileiii 1934.) 

Cl wt. Perctnt IM c^ R oM ^5^,.,!L, ptr , J2SLW:. .*?*, ."*AY*}!*.*iL ^ 

in Solvtftt " "^ W tfi ?.^> 

87.7 0.1095 < 

92,6 o.oa86 o.o ^H o.c 

o5 . $ 0*007H OfcOOHtj O.OIO^ 

!0o.o o.oojr6 o.cicia? 0.0029 

SOLUBILITY or POTASSIUM CntoRioi IN AQUEOUS SOLTIONS or 

TlITlARY BtJTAWL AT ;|0 . 
fOknnint a %! nx>%> 

The results which were determined by ib* *iyRth*tic eibod locate the 
binodal curve of the system anil incittrtf li^ lints * which how the 
composition of layers in contact with e*ets other And the pUtt point, 
PP, at which the two liquid layers homogeneous. 

OKA, par 100 m* *t. aol. flfc*. Pf WO fit. U iI !. fif WO jpa. MC. 0i. 



' ^3)3 


m ^ ^I S UK 




^f <!(<>, TOM Wl 





33*1* J*3 


H.I 


19,0 4.2PP 


7.9 


15.9 ao.^ 


7. it 


1 * H 1*1 


9.4 


14.6 


7.4* 


^Q*g a.6 


10.5 


13.3 


6*7* 


5 '1 . o " 


ll.S 


12.2 3V 


6, i 


57*0 


12. < 


11.4 ^*S 


'.6 


|B,ft 2.0 


16.5 


9-0 11.1 


4.B 


67.1 l.tt 9 




16.6 


*l. 


OO.O "" 



The composition of the plait poini.PP, AI js tf in 11.5 8^ KCl and *ii.o 
gms. <CR 3 ) 3 OOH per 100 gm. SAI, solution, tunning**, Herring Anl 
Webb, 1933. 



779 

DISTRIBUTION OP POTASSIUM CHLORIDE BBTVBEN WATKR 
AND BUTYL ALCOHOL AT 25. 

(Alleaan, 19^8.) 



KALIUM K 



Normality^pr KC1 in: 


(b) 
k (a) 


r H g O layer (a) C^OHfb) layer ^ 


2.0 0.0182 


0.0091 


i.o 0.0134 

0.50 0.0079 


0.0135 
0.0167 



Normality of KC1 in; 
H g o layer(a) C 4 H Q OH layerfbp 



0.25 
0.10 
0025 



0.0051 
0.0020 
(O.OOll) 



(a) 

0.0199 
0.02O4 
(0.0455) 



DISTRIBUTION OF POTASSIUM CHLORIDE AT 17 BETWEEN : (Wosnessonsky, 1025.) 
Water and Amyl Alcohol. Water and Phenol. 



MilUmoLs. KCl per liter of 

H 8 layer iCx). Alcohol layer (C,). 

36o.*55 o.83i 

5i2.oii i.oSo 

677.607 1.287 

810.000 1.491 

921.140 1.648 



c 

q-' 

461 
480 
486 
478 

477 



MllUmols. KC1 per liter ( , 

H a O layer iC t ). Phenol layer (C,l. <* 

64.0 4.5 14.2 

in. 5 7.9 14. i 

290.3 o.4 14.2 

3*4.5 aa.8 14.2 



SOLUBILITY OP POTASS run CHLORIDE IN ANHYDROUS ACBTIC ACID 
DBTBRMINBD BY THB SYNTHBTIC METHOD. 

(Dttvldson and Chappell, lose.) 



GM. Hols. KC1 per 100 on. aola. 
c KC1 CH^COOH 

16.45 0.168 

24 0.157 

30 0.170 

39 O.l88 

U7 0.207 

55 0.229 



Solid 
Phase 



CH 3 COOH 

KC1 



On. Hols. KC1 per 100 pa. nols. Solid 
KC1 4 CHCOOH Phaat 



59 

63 
70 
76 
87 
93 



0.239 

0.257 
0.272 
0.295 
0.336 
0.367 



SOLUBILITY OF POTASSIUW CHLORIDB IN AQUKOTTS 
SOLUTIONS OF URBTHAM AT 25. 

(Pall each, to?9. 19?9.) 



KC1 



Dm. Hols, per 1000 gma. H ? 



NH 2 TOOr. ? H s 


KCi ^ 


0.0 


^.83 


0.056l 


4.81 


0.0786 


M.8o 


0.2245 


4.76 


0.5612 


4.66 


1. 1225 


4.49 



Solid 
Phase 



KC1 



On. Mola. per 1000 

-r 



2.597 
3.972 
27.556 
28.477 
40.88 
53.09 



H0 



3.84 

2.20 

2.0 

i.o 

o.o 



Solid 
Phaae 



KCl + NH 2 COOC H B 
Lower liquid layer 



Upper 
NH ? QQOCH 



25 



loocc sat. sol. of potassium chloride in ethyl urethan 
contain 0.105 m KCl at 60. (Stuckgold, 1917.) 



K KALIUM 

SOLUBILITY OF POTASSIUM CHLORIDB IN AQUEOUS ACKTONK SOLUTIONS. 

(Sncll, 1898; at *, Hen awl Knoch, t*oi,) 



Wt. (see Note) ^,. At M - 
Percent KUncrioocc. 
Acetone in Solution. 


At jo w , 
Cms, t*er ice C 
Solution. 


Jms, 


At 40*. 
Cms, per 100 (rim. 
Solution. 


At jo*. 
Cms, ier 100 Cms. 
Solution. 


Solvent. 


Millimols. 


Gnu. 


Acetone, 


KU. 


Acetone. KC'I," 


Acetone, KCir 





4IO 


5 


30,62 


O 




27. 


27 


o 28. 6c> 







30 


9.1 


35* 


7 


26.23 


6 


-96 


23- 


,42 


6-79 25.33 








20 


286 


.6 


21.38 


16 


.22 


18, 


go 


IS.75 21. 28 








30 


223 


7 


16.69 


25 


45 


X S' 


,06 


two layers 


25 


.67 


14-42 


40 


166 


S 


12.42 


35 


.52 


n, 


31 


44 


36 


.03 


9-93 




115 


4 


8.61 


45 


.98 


8, 


,04 


(4 


46 


,46 


7.07 


60 


71 


.2 


5-3* 


56 


.91 


S 


.12 


II 


57 


37 




70 


38 


-5 


2.87 


68 


.18 


2, 


,60 


it 


68 


,56 


2,22 


80 


12 


9 


0.96 


79 


43 


O, 


,76 


70.34 O.S8 


70 


^5 


0,04 


90 


2 




0.15 


89 


.88 


O 


13 


Bc),B4 0.16 


dU 


^ * o 


sat. sol. 



100 O O IOO O IOO 



NOTE. For the 20 results the per cent acetone in the solvent in in terms, 
of volume instead of weight pcr cent, and the concentration of the second solu- 
tion is 10 per cent instead f 9.1 which is the weight |>er cent concentration of the 
solvent for the corresponding results at the other tenipcr&turoa. 
Cl 



AT THE TEMPERATURE 40 AND FOR CONCENTRATIONS or ACETONE BETWEEN 20 

AND SO PER CENT THE SATURATED SOLUTION SSPAKATKS INTO TWO LAYERS 

HAVING THE FOLLOWING COMPOSITIONS: 

Upper Layer. Lower layer, 

Cms. per 100 Cms. Solution. Cim. per too CJmn Solution. 

iHaO. (CH^ 1 CcT~"''"ix : i^ ^HjoT' ' (Ciy,(tK "" KU 

55-2 31.82 12.99 28.14 6^,42 2.44 

53-27 3S-44 xi. 29 30,96 65.97 3,07 

51.23 48.50 10,27 32.64 63.79 3,56 

5-34 39.88 9.77 34.07 62,01 3,92 

48.02 43.18 8,79 37.44 57,67 4^ 

46.49 45-34 8.17 38,68 56,17 5.25 

58.99 25.24 15,77 23,66 74,91 i ,43 



^, No solid phase could be present when equilibrium is attained 
since, with vapor, there are 3 components and 4 ph*e; Nenc^ iJt the 

temperature is fixed the system becomes invariant,. 

loo cc. sat. solution of potassium chloride in furfurol (CJIiO.COH) contain 
0,085 gm. KC1 at 25. (WaUkfl| I9o60 

1000 gms. highly purified lucetone dis.wlve 0.00087 g. KCi 41 i8 and 
0.00097 gm. at 37 as calculated from specific conductivity measure- 
ments. (Lannung, 1932.) 



7 8l KALIUM 

SOLUBILITY OF POTASSIUM CHLORIDE IN DILUTE AQUEOUS SOLUTIONS OF 
SEVERAL COMPOUNDS AT 25. 

(Armstrong and Eyre, 1913.) 

Gms. Cmpd. Cms. KC1 Cms. Cmpd. Gms. KC1 

Comoound. per 1000 Gms. per 100 Gms. Compound, per 1000 Gms. per 100 Gms. 

HA Sat. Sol. H 2 0. Sat. Sol. 

Water alone ... 26 . 89 Glycol 15.51 26 . 43 

Acetaldehyde n.oi 27.05 " 62.05 25.26 

Paraldehyde 11.01 26.42 Mannitol 45.53 24.86 

Glycerol 13.01 25.58 " 136.59 24.46 

100 gms. 95% formic acid dissolve 19.4 gms. KC1 at 19. 7. (Aschan, 1913.) 

44 glycerol (d {6 = 1.256) " 3.72 " " "15-16. (Ossendowski, 1907.) 
ioo cc. anhydrous hydrazine " 9 " " " room temp. 

(Welsh and Broderson, 1915.) 
ioo gms. hydroxylamirie " 12.3 " " " 17-18. (de Bruyn, 1892.) 

SOLUBILITY OP POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OP GJLYCOL AT 30 

(Trimble, 19551.) 

d. of 08. per 100 jpa. aat. sol, 

sat. sol. 

1.1820 

1.1648 
1.1510 
1.1424 
1.1371 
1.1368 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF GLYCEROL AT 25*. 

(Herz and Knoch, 1905.) 
Sp. Gr. of Glyceroi at 25/4 = 1.2555. Impurity about 1.5%. 



CH^OHCH^OH 


KCl 


0.0 


27.10 


15.08 


21.97 


33*47 


1^.53 


52.00 


11.84 


73-37 


7.75 


94.90 


5.0O 



Wt. Per cent 
Glycerol in 
Solvent. 


K.C1 per ioo cc. 
Solution. 


Sp. Gr. of 
Solutions. 


Wt. Per cent 
Glycerol in 
Solvent. 


KC1 per ioo cc. 
Solution. 


Sp. Gr. of 
Solutions. 


JVlillimols. 


Gms. 


Millimohi. 


Gms. 


O 


424 


-5 


31-66 


I. 


,180 


54-23 


238, 


5 


17, 


79 


I.2I9 


I3-28 


383 


4 


28.61 


I, 


.185 


83.84 


149 




II 


.11 


1-259 


25.98 


339 


3 


25-3I 


I, 


.194 


IOO 


110. 


.6 


8. 


25 


1.286 


45-36 


271 


4 


2O.24 


I 


.211 















ioo gms. HaO dissolve 246.5 gms. sugar + 44.8 gms. KC1 at 31.25, or ioo gms. 
of the sat. solution contain 62.28 gms. sugar -f 11.33 gins. KCl. (Kahkr, 1897.) 



SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF GLUCOSE AT 25* 

(Armstrong and Eyre, 1910-11.) 



Wt. % 


Gms. KCl 


QHna+EW) 
in Aq. Solvent. 


per ibo Gms. 
Sat. Solution. 


O 


26.63 


4.72 


25.86 


9 


25.18 


16.53 


23.89 


37-27 


20.15 



K KALIUM 782 

SOLUBILITY OF POTASSIUM CHLORIDE in AQUEOUS SOLUTIONS or DIOXAN AT 25. 

/IJ*K And lurenta. fMK&-\ 



Vol. Percent *>. MOl. KCl Vol. Ptretnt 0*. Mol. KCl 

Dloxan in Solent P*r itwr mt. ml, Oioxw la olvtnt ptr lUtr a&t. sol. 

10 3*45 $5 0.8$ (L) 

20 2-80 77 0.14 (U) 

33 2*00 80 0.12 

5 K22 

Between $1 and 77 Vol. percent Dioxan to liquid layers are formed 

(L) s lower liquid layer tU) s upper liquid layer 

SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OK PYKIDINB AT 10*. 

(Scbroedr 1908.) 

Aq. Mixture. ^* mSl ^ At|, Mixture. ^nwi. KCl 
"-M * v *r >i r u **' > _ jytr ioo Gm. .^^.^.J^.^.^. ..!.... . t*.* i<^ tim* 

SllA cc. Pyridine. *^S*$8T iO- ce. Pyridine. 



ioo o 23.79 40 60 3,33 

90 10 19.76 3<> 7 1-25 

80 20 l6,37 20 SO 0,24 

70 30 13.19 10 go 0,04 
60 40 10.05 o ioo o 

50 S 6,34 

The binodal curve and plait point of the system KCl * Pyridine * H f O 
at 25 has been determined by Ginnings, Webb and Hinnh&ra, 1931, but the 

authors do not give their experiment*! results but only the values of a 
series of arbitrary constants calculated irm them by weans of empirical 
equations. 

ioo gms. HOP id Sulfur Dioxide dissolve o*on* P* KCl at o. (Jander 
and Ruppolt, 1937. I 

ioo gns, sat. sol. of Potassium Chloride in Selenium Oxychloride 
contain 2,89 gms. KCl at 35. {Wise, 



PUSIOH-POINT DATA HAVE Bitfw DITIRHIHI ro THE 

FOLLOWING Mxrraitta OF KCl AH ft OTKIK SALTS. 



KCa t KI (iMa)(3) KCl 4- K ? S0 4 t 3 HsH7l KCi * Nad (3)(8Mn)(ia) 

* KOH (4) H * " * NaCl Ci8) * WaJKMB) 

i irpw/v I M n f A i * ttt rl 

" + KPO 4 (6) " * HgCl f (81 * SUCI. 

HH!NO,. 



I MaCl 



4 ^ 4 3 " ^TlCl Ho) 



d) Wrxesnewski, 1912; la) Ammtori ad Pampanini, 1911; 

Plato, 1903; (^) Scarpa, 1915; (5) Sackur, 1911-13; <6) n^tor, 19x2! 

(7) Janecke, 1912; (8) S&ckur 1913; <9l Vorii%ch, 1914; Uol Haadonnini, 

1911; i9i<; <"* Schaeffer r 1919; (12! UutHbrry and Page, 1920; 

(13) Scholich, 1920; (14) Perman and Saunters 1933; ^15! Jtmecke, 1938; 

(i6)Menge, 1911; (17) Derby t 1918; (18) Richards' And Heldmro, 1917; 

(19 Keitel, 1925; do) Kendall, Crittenden mil Miller, 1923; lai> Elchardus 

and laffitte, 1932; (22) Keitel, 1925; 133) Zouravlev, 1939 1 2*4) Waxberg, 

1930; (25) Zemcznwiy, 1908. 



783 

POTASSIUM Palladium CHLORIDE KJPdCl. KALI DM K 

o 

From measurements of the solubility of Potassium Chloro-pallaciate 
(K^PdCl fl ) at 25 in normal aqueous Hydrochloric Acid containing KC1 and 
saturated with Chlorine at atmospheric pressure the Solubility Product 
(K+ ) ? (PdCl e ~" ) was found to be 5.97 x lo"" 6 moles per liter. (Wellman, 1930.) 

POTASSIUM Platinum CHLORIDE See PLATINUM CHLORIDES 
POTASSIUM Rhenium CHLORIDE K ? ReCl e 
POTASSIUM Rhenium Oxy CHLORIDE K 4 Re 2 OCl 1) 

SOLUBILITY OF EACH SBPARATELY IN AQUEOUS HYDROCHLORIC ACID. 

ana Noddak, 19,^.) 



Wt. Percent KC1 0ms. K^PcCl- pr Oms. 

In AQ. Solvent lOOOcc sat. solution at: lOOOcc sat. solution at: 
^, .^^^ ^^^-^ ^. .^^s^^p.^ 

12.0 21.38 30.28 750 

20.0 2$0 46.0 

37.0 33 3-72 5.5 

Mono POTASSIUM Tin CHXOKIDE KSuCI 3 .H 2 0. 

SOLUBILITY OF MONO POTASSIUM STANNO CHLORIDE IN WATER. 
(Rhubarb und Fleck, 1916.) 

t" ................ "<\,'2, u". 2. :n",B. so*. 4. 71". o. 

Gms. KSnCl 3 per 100 gms. sat. sol ---- 2(5. i 34-9 54o 72.8 8->..i 

Solid phase K Sn Cl 3 .H a at all temperatures. 

Di POTASSIUM Tin CHLOKIDE K 2 SnCl*.2 H 2 O. 

SOLUBILITY OF Di POTASSIUM STANNO CHLORIDE IN WATER. 

(Himbuoh and Fleck, 1016.) 
Gms. per too gms. sat. sol. ^^^^ 

Solid IMiaso. 

K 2 SiiCU.?H 2 



t". 


01. 


Sn. 


K. 


K s SnCI 4 . 


2.3*.. 


9. 14 


3.28 


7.9'1 


- 


14.1*.. 


12.18 


5.68 


9-7^ 


- 


35.6... 


18.28 


+- 14. 56 H- 


10.61 


= 43.5 


5 7 ./i... 


23.t3 


-H 19.50 H- 


I 2 . 7?. 


=. 55.4 


77-3.., 


26.56 


+- 22.35 H- 


14.63 


= 63.5 



Tetra POTASSSIUM Tin CHLORIDE K 4 SnCI.H 2 0. 

SOLUBILITY OF TETRA POTASSIUM STANNO CHLORIDE IN WATEB. 
(11 unhitch and Flock, 10 10.) 

Gms, per 100 gms, sat, M>|. 

K A Sn<:iT. Solid Plmse. 



t". 


Cl. 


Sn. 


iimmaar 

K. 


o.5*. . 


10.99 


0.93 


H.55 


19.5*. . 


i3.io 


i .i)3 


13.19 


4i.o*.. 


16,00 


5.82 


i3.84 


61.7*.. 


20,18 


9-95 


15.73 


70.0. .. 


22.71 H 


12.86 -H 




81.2... 


25.74 -t 


- 19.57 -4- 


15.71 



= 61.02 

* At thosts temperatures tho atomic ratios in solution did not correspond to tho douhl* sail h*no 
the solid phase in a mixture of the double Ball and lntmo <*hlori<lc. 

Experiments on the Solubility of Potassium Stannic Chloride and Ammonium 
Stannic Chloride in Aqueous Solutions of Hydrochloric Acid containing 
sodium and ammonium chlorides are given by Smith, 1928. 



K KALIUM 



7811 
or POT ASM UN CM 1.0* A r IN WATKR. 



The results of Taylor, iB^ji Carlson, mn; OiUoUn, 1913; Brdnsted, 
1013; Tschugneff and Chlopin, 19 u* TVvU, 1931, 1933; lijinskl, i$ 32 ; 
Wright, 1927; Hi Capua and Scalleiti, i|j?; Flttumann, 1938; Ricci, 1937, 
1938; and Ricci and Yanik, 1937* w ***e fiUmed md ilie following average' 
values read from the curve. The result* abtw* 100 are from TiUen and 
Shenstone, 1881; and Ben rath, (yertebo, Schiller** And Wunttarlich, 1937. 
The solid phase is KClO^ ia All 



Of Oft 

sol. 100 



100 pit. Ml. 






1 


.031 


3 


2 


70 


31. 


a 


300 


72 


.0 


10 









9 


80 i iM 


37* 


:i 


330 


78 


.0 


15 


( i 


.0363) 


5* 


7 fs73$l 


90 """ 


|i. 


S 


3 no 


Us 





20 


(1 


,0^20) 


6* 


8 {6,793! 


1 00 1 i 1 9 


16* 





360 


87 


.0 


2$ 


(i 


.0^8^) 


7. 


9 (7.999) 


I04b*f l3 JO 


17. 


5 


380 


91 


.0 


30 







9. 


a 


1 3d ***** 


l V 


s 


300 


94 


5 


40 


i 


073 


12. 


3 


uo 


53* 


o 


,110 


96 


7 


SO 







s* 


6 


160 


59- 











60 


i 


.115 


19. 


2 


180 


IH, 












The results ia parettihests are by Pittit*ann itaS. 

CIO SOLUBILITY OF POTASSIUM CHLOKATR IN AQUHOUH SOLUTIONS 01 

POTASSIUM CHLOHIDK AT 3o fl , 



5p. Or. of 


Onms 


J2-HS^% ^ 


. <*r. *if 


*;?4w 


iw Uiw. 


Solutions. 
.050 


O 


IBS s 
71.1 


.098 


110 


24-5 


.050 


ID 


58-0 


. loi 


140 


23 5 


.050 


2O 


49 o 


. 119 


tfto 


21.0 


.054 


40 


39 -S 


MO 


180 


10-0 


.064 


60 


34 -0 


.140 


300 


J0.0 


1 S 


80 


30.0 


.168 


250 


20-0 


1 .086 


100 


27,0 









*SOLUBILITY OF POTASSIUM CHLORATE IH SOLUTIONS Of 

POTASSIUM NITRATE, 

t Z 1 1 # 397* V J ) 



Results at 

Mais. p;r Uwr. 


Offtm* prr t..itrr> 


Resiilti 

Ml jw t jirr 


lit 23.S7 , 
OwiwrOtfr. 


Kt 


O 
O 

I 
a 


^Os. 
.0 

.125 
.25 

o 
.0 


K- 

o 
o 






.570 

529 
.492 

374 
.328 


*M 
O' 
12 
25 
101 
202 


O 

.6$ 

,29 
.19 


kCit,% 
6g.88 

64.86 

^33" 

4S'% 
40.22 


^- .*^^^ 

o-o 0.645 

0,$ 0.SI5 


o.o 79 

50,59 6j 


,09 
,14 



?85 KALIUM K 

APPROXIMATE SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SALT SOLUTIONS 
AT SEVERAL TEMPERATURES. (Alekccevsky, 192 1.) 

The determinations were made by adding K Cl 8 to the aqueous solvent untill 
no more dissolved after a period of 3 hours. The curves drawn from the results 
are very irregular, thus showing that saturation could not have been reached in 
all cases. 

Cms. KClO a per 100 cc sat. Solution in Aq. icons. 

o KaCoT""^ /o K* COTuoVft K s CO, 40 /o K a *'0 a . 

4.0 2.5 2.0 

5.o 3.5 2.5 

6.5 4.5 4.5 

7.5 6.0 6.0 



f. 

20. 

40. 



/oK 5 C0 3 . 

6.0 
6.5 
8.5 
9-5 



O 

6.0 
8.0 
9.0 



0<V K a C0 3 . 
I .() 
2.5 

3.5 
4.o 



Cms. KClOj per lOOcc sat. Solution In Aqueous. 



t*. 

2O . 


5 to 7 /o Na s C0 a . 
5.o 


5 / Na Cl. 

5.o 


30/,NaCl. 

5.o 




5.5 


5.5 


5.5 


/o 


7.5 


7.5 


6.5 


5o 


io.5 


i3.o 


n. 5 



Gm. mols. per liter. 
ROB/ ^ KCtOj. 

4.71 o . 0924 

5.06 0.0882 

6.35 0.0609 
7.95 o.o445 


Gm. mols. per liter. 


KOH. RC1 3 . 

8.60 o.o4io 
9.41 o.o35i 
10.95 0.0287 
12.19 0.0254 



SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM HYDROXIDE AT 20. ( Brims ted, 1020 a.) 

Gin. mols. per liter. 
KOH. K.C1 G 3 . 

1 4 02 O . O2 1 5 

i 4- 85 0.0195 

ij.oa 0.0191 

SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF POTASSIUM NITRATE 
AND VICE VERSA AT 25. (Toda, 1021 a, ma.) 

Saturation was secured by constant rotation in a thermostat. 

Gms. per 100 guts. sat. sol. 
KN07 

18 97 
27.14 
27.14 
27.21 
27.57 
27.7.4 

SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORATE 



C1C 



Cms. per 100 

- ^H 


gms. sat. sol. 


Solid 


UNO,. 


^ KCIO^ " 


Phase. 


O.O 


7-745 


KC1 3 


0.68 


7.65 


KC10 3 .N0 3 


i.55 


7.07 





3.59 


6.52 





7. 12 


5.76 





12. 8t 


5.i<> 






us. SHI. si. 


Solid 


KCIO,. 


Phas. 


4.39 


KCI0 3 .N0 3 


3.9<) 





3*90 


KClO 8 -4-KNO 


3.6i 


KN0 3 


i.63 





0.0 






AND VICE VERSA AT St4.2. 
See note under Potassium carbonale, 

Gms. 



AT 40. (Iljinsky, 



f- 8 


at. sol. 


NaC10 3 . 


KC10 3 . 


OU1UI. 

Phase. 


24.2. . 


.045 


0.5 


8.1 


KCIO, 


. . 


.086 


7 .5 


8.0 





. . 


.189 


2 7 .5 


7.0 





. . 


.24l 


4i .0 


6.0 





. . 


.260 


47-4 


5.o 





. . 


.326 


60.0 


5.2 


v) 


. . 


329 


61.8 


5.6 





. . 


.392 


82.7 


5.3 






OiU8. 


per 100 gin 8. 11*0. 


d of. 


*" ^W-^s. 


--*^---^. 


Solid. 


lat. hoi. 


NaClOj. 


KC10 8 . 


IMui^o. 


.441 


99-7 


3. i 


KClOj-hNaClO, 


.42<) 


98.6 


O.O 


]N'C 1 a 


.073 


O.O 


i<.a 


KC1 (> a 


_ 


i3.5 


9-9 





.268 


48.4 


7.0 





.3o8 


58. 7 


7.0 





.453 


98.8 


7.0 





.483 


nC.o 


7.2 


4-NaClO, 


.462 


116.4 


0.0 


NaOlO, 



K KALIUM 

SOLUBILITY OF POTASSIUM CHLORATE TN AQUEOUS bOLUTiONs OF POTASSIUM 
HYDROXIDE, HYDROGEN PEROXIDE, AND MIXTURES OF THE Two AT 25. 

(Calvcrt, 1901.) 

The mixtures were agitated by means of a stream of air. Equilibrium was 
approached both from above and below 25. 

Mols. KGOa Cms, KCI0 3 

Composition o[ Solvent. . Dissolved per Dtaolved per 

Liter of Siit. Sol. Liter of Sat. Sol. 

Water alone - 6 7S 82.71 

Aqueous o.r 25 n KOH - 62 S ?6.6o 

" 0.2$ n " 0.573 70.23 

Aq. HjO* containing i . 26 mols. HA per 1. o . 730 $9 . ^5 

" " 1.31 0.737 90.33 

Aq. 0.25 n KOH " 0.015 0.578 70.82 

" " 0.276 , 0,584 71,57 

" " 0.954 0.616 75-50 

" " 1.073 0.673 82.47 

SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS or 
POTASSIUM BROMIDE AT 13. (Bkr, ion.) 



Cms. per too Gins. 
Solution. 


Cms JHT too Gmsi. 
Solution. 


Gitm. i XT TOO Cms. 
Solution. 


'KBr. 


KClOg. 


'KBr. 


KClOi. 


'KBr, 


KOKV 


O-2O 


S .l8 


I .O 


5*04 


6.0 


3.46 


0-6o 


5.20 


2.O 


4.60 


S.o 


2.8o 


0.8 


5-o6 


3-<> 


4.2 


IO.O 


2 .40 






4-0 


4-0 







CIO 



SOLUBILITY OF POTASSIUM CHLORATE IN AOUEOUS SOLUTIONS OF OTHKR 
POTASSIUM SALTS AT I4 & -I5 . (ftlarcx, *<)**,) 



Gms. per 100 Cms. Solution. 



OillL. / 


K Salt. 


KUOi. 


KOH 


1-43 


4-47 


KC1 


I.9X 


4-45 


" 


3.82 


3 -5* 


KBr 


3.05 


4.49 





6.10 


^,60 


KI 


4.25 


4-59 





8.51 


3.65 



Salt. 

KNO S 



Gnu, per too OmR. Solution. 
' ifShu 



KAO* 



5.18 

4.46 

2.42 
4.85 



4.51 
3.88 

3'9 
3-93 



SOLUBILITY OP POTASSIUM CHLORATI i Aywious SOLUTIOWS or 
SIVBRAL SALTS, EACH DITRRMIWSD StPA4Titt AT 35, 

(HoUutA ana Peter, I )?*).) 



Concentration 

of Aq. Solvent In 

Ow. Equlv. Suit par litr 

0.0 
0.02$ 
0.0$ 
0. 1 
0.2 
0.3 
0.4 
0.5 
0-75 
1.0 
2.0 
3*0 
4.0 
5-0 



per lUr Mt. solution in 



;>olutlono or: 



' Ktl 


m^ 


~"V4 




"^*ssr^ 


83*030 


83.030 


83.030 


83.030 


83.030 








82.570 





- 








80.622 


. 





76.653 


77.951 


79-103 


76.974 


83-333 




75-225 


7S-3S7 


71-959 


84.383 


67.793 


72.587 


71-995 


67.655 


85.615 


64.191 


70.346 


6^.834 


63-805 


85-998 


60.375 


68.695 


67.004 


60,027 


86.968 


Sn . o 10 


63.619 


59* y*9 


^3.208 


88.069 


t\B. 142 


61.096 


<|| r jfU* 


49 -170 


88.924 


34-673 


$3-^13 





40*42$ 


90.398 


27.600 


119-068 





33-300 








. 





32,228 






7 8? KALIUM K 

SOLUBILITY OF POTASSIUM CHLORATR IN AQUEOUS SOLUTIONS OP 
POTASSIUM IODIDE AT 25 AND VICE VERSA. 

(Rlccl, 1937.) 



of Qtes* P* r ^00 8* aat 9 l - &OLIQ d. of fta. per 100 
sac! sol. ' KCIOI KI ' Phase sat. sol. 



1.047 


7.905 


0.0 


KCIO H 


1-555 


1.10 


1. 103 


5*04 


9.33 


M 


1.702 


0.82 


1.178 


3-35 


18.74 


M 


1.724 


0.83 


1 . 275 


2.30 


28.72 


M 


1.724 


0.67 


1.400 


l.6o 


39.26 


II 


1.718 


0.0 




SOLUBILITY OK POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM TODATE AND VICE VERSA. 

(Riccl, 1938.) 

Results at 25 Results at 50 

d. of (tas. per 100 ^gms. sac, sol. Solid QMS, per 100 JB. sat, sol. Solid 

aal . sol. ' Kft^ * WXS^ v Phase / KTO"^ "KCHJ,, v pnas* 

1.048 o.o 7.90 KC10 3 o.o 15.78 KC10 5 

1.068 2-92 7-31 " % 2.41 IS-" " 

1.090 5.43 6.80 " KI0 3 5.27 14.31 " 

1.082 5.85 5-31 KIO,, 7.27 13-77 " + KI 

1.070 7.05 2.31 " 8.76 8.58 KI0 3 

1.043 8.45 0.0 " 10.87 3-71 

13.21 o.o " 

SOLUBILITY OP POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS op 
POTASSIUM SULPATE AND VICE VERSA. 

(Rlccl and Yttnlck, 1937.) 

d. of Oftm.. per 100 pts. sat. sol. Solid d. of 0s. per logins, sac, sol. Solid 

at. sol. ' RWd,, A ff^j ^ Phase sat. sol. ^ fTCIi^j KJSCf^ ^ Phase 

Results at 15 Results at 25 (con.) 



1.032 5.676 o.o KClO, 1.100 4.96 8.64 

1.085 3.29 7.86 " + ^2^4 1.099 3-30 9*43 
1.076 o.o 9.258 K g S0 4 1.089 1.80 9.93 

1.083 o.o 10.76 
Results at 25 

Results at 45 

1.048 7.897 o.o KCl0 3 

1.063 6.72 2.73 " 13-90 o.o KClO, 

1.080 -5-77 5.57 " 9^8o 9-13 " + *?4 

1.099 5.06 8.19 " ~" 0.0 13.53 K P ^0 4 

looocc aqueous 5.2 percent NH^ Solution dissolve 52.5 gms 
at 20. (Konowalow, i899b) 



K KAL1UM 

SOUWUYY or POYAIWH t* SOLUTIONS or 

*** CM tOft AY* A*f> VlC* AT jo**. 

ii. 



CIO 



The pile irregular resuiiJi of ihf .tuihor* w*rr jhui*ii And the fol- 
ava value* frtm ttt* tiwrvt. 



lowing average value* frtm ttt* 



TIOT, 



6.75 

it .6 
3.8 



0*0 
5-0 

10.0 



KCIO,, 



i&Solmt. gotutiaiu 

o 9.23 
5 ?? 



xo 
20 

30 
40 

50 
60 



90 



In Aqueous Alrohnt 

p^-* , T , - Al 

At w*. At , 



13 ;tf 

JO 4^ 
K 84 
6 40 
4 67 
3 4t 
a 4t 
i 41 
o ?J< 
o jl 

t> U 



6*44 
4-51 



1,64 
1.01 

0,54 
0.24 
0.06 



10 17 
8,80 

S 90 

4<74 
4.00 

3 3.1 
a 53 
iJat 

I .21 

o.&a 



***, tr 



j.u 

I, n 
o, 11 
o.o 



\\ #l/ 

13 ( )3 

IP 77 
H j6 

5 HH 
4 I4 
1 ^) 



J 



^ii?!IJ~ 
no. a KClO, 



toita 



HJ.O 



1 ; 

Al i * 
t Ktl 



<) ^.l 

|J 

? ftj* 

4 Oi 

J H> 

j qo 

2 ll| 

i 14 

o 57 

o iH 



H 10 
1 40 
6 76 

S l l 
I iH 

j HE 



HCIO. 



Uiiw, 



At 40*. 



13,23 

II 10 

10 ^8* 
B-j 7 
6-6c> 

$3* 

4 0,1 
3 B6 

i -wi 

o 79 
0-^4 



12.60 

11,26 
10.34 

9-4$ 

8.40 



S 

3 '97 
245 



loo 



at 
ubet. 






gus. 
ia 



Tht 



by 



10 



r CtUMUYt in 

or 4? i? i*. 



it 



ti! 



MI! m 



! 



0*0331 



789 



KALIUM K 



SOLUBILITY OF POTASSIUM CHLORATE IN 
COMPOUNDS AT 25. 



AQUEOUS SOLUTIONS OF VARIOUS 

(Rothmund, 1910.) 



Aqueous 0.5 Normal 


KC)0 3 per Liter. 


Aqueous 0.5 Normal 


KCIO a i>or Liter. 


Solution of: 


Mols. 


Gins. 


Solution of: 


Mols. 


Gms. 


Water alone 


O. 


1475 


20, 


44 


Ammonia 


0. 


,1474 


20.43 


Methyl Alcohol 


Q. I4O2 


19, 


43 


Dimethylamine 


0. 


1342 


18.60 


Ethyl Alcohol 


0. 


1356 


18. 


75 


Pyridine 


0. 


1410 


*9-54 


Propyl Alcohol 


O. 


1343 


18. 


61 


Urethan 


O. 


1400 


19.40 


Tertiary Amyl Alcohol 


0. 


1279 


17. 


72 


Formamide 


O. 


1539 


21.32 


Acetone 


0. 


1451 


20. 


ii 


Acetamide 


O. 


1447 


20.05 


Ether 


0. 


1336 


18. 


51 


Acetic Acid 


O. 


1462 


20. 26 


Glycol 


0. 


1416 


19. 


62 


Phenol 


O. 


1362 


18.87 


Glycerol 


o. 


1404 


19. 


45 


Methylal 


O. 


1400 


19.40 


Urea 


0. 


1510 


20. 


92 


Methyl Acetate 


0. 


1429 


19.80 



SOLUBILITY or POTASSIUM CHLORATE IN GLYCEROL. 



d. Of 

u Olycerol 


Percent 
Olycarol 


15-16 
20 
20 


1.256 
1.2326 
1.2645 


96.0 
86.5- 
98.5 


25 


1.249 


95.0 



Ctoa. 

100 O 



KQO per 
B* glycerol 



Authority 



3.54 (Ossendowski, 1907.) 

1.32 (Holm, 1921, I92i(a), 1922.) 
1.03 " " " M 

1.05 (Schnellbach and Rosin, 1931.) 

100 gms. sat. solution of KC10 3 in glycol contain 0.9 gm. KC10 3 . 

<de Coninick, 1905.) 
100 gms. liquid ammonia (NH^) dissolve 2.52 gms. KC10 3 at o . 

(Hunt and Boncyk. 1933.) 
POTASSIUM Per CHLORATE KC10 4 

SOLUBILITY OF POTASSIUM PBRCHLORATB IN WATER. 

The following values were taken from an average curve constructed from 
the results of Pierrot, 1921; Willard and Smith, 1923; Moser and Ritschel, 
1925; Flbttmann, 1928; Cornec and Neumeister, 1929; Flatt and Jordan, 
1930, 1933; anc * Caven and Bryce, 1934. Above 100 Benrath Gjedebo, 
Schiffers and Wunderlich, 1937. The results in parentheses are the 
average of previously reported determinations by Carlson, 1910; Rosenheim 
and Vfeinhaber, 1910-11 and Calzolari, 1912. The solid phase is KC10 4 in 
all cases. 



o 
10 
15 
20 
25 
30 



d.of 
sac. 
aol. 

1.005 

1.0O76 
1.0085 
1 . 0096 

(1.022) 



per 100 ana. 


t 


aac. aol. 




0-75 


so 


1.05 


60 


l33 


70 


1.65 


75 


2.03 


80 


2.50 


90 


3.60 (4.4) 


100 



d. or 
sat, 
aol. 



Otta. KC10 4 

per ICO ess 

aau aol. 



1.017 a 90 

(1.033) 68 



(6.5) 120 

(9.0) 140 

111. 81 l8o 

1.036 10.36 200 

(1.053)11.8 (14.8) 225 

is.o (18.0) 250 

I.o68ll8.2 (21.8) 265 



daft. KCLO 

per 100 pi 

aau aol. 

25 
32.5 

46 

52-5 
60 
67 

70 



KALIUM 790 

SOLUBILITY or POTASSIUM PERCHLOKATK IH AQUEOUS 
SOLUTIONS op HTTMOGIH PEROXIDE AT 25 

(Antrlor and "tore*, 1935.) 

**** H^O^ pr Cte, Hols. KflO ptr 

IOC w** aq. solvwt looe 911. aq. jvt*u 

0.00 0,1149 

15.72 0.175 

SOLUBILITY OF POTASSIUM PERCHLOIATI in 
SOLUTIONS op ALUMINUM PERCIUORATS AT 30 

(Cr&vtft ami ftiyci, WS4.) 

(tea, ptr 100 jp.. H^ Solid % ptr 100 

i A1(C10 4 ), rClO. A PtitM 



o.o 2.528 KCIO^ 4.956 i. 03 a KCIO 

2.652 i.i6a " 8,158 0.70*11 H 4 

3-043 1.357 " 314.56 0.2115 rl 

SOLUBILITY OF POTASSIUM PBRCHLORATE IN AQ. KCI AMD AQ. Ktft 

SOLUTIONS AT 25**. (Noyaal BOM*, 1911.) 



In Aq. KCI Solutions. 
Cms. per ico.a cc. Sat. Sol. \ 


IVt. of 10. a cc. 
of Solution. 

IOI.42 
101.45 


In 

Om, per loo, j 


Aq. KiSO, 
cc. Sat! Siil, 


KC10 4 . 
2.0566 
1.7800 


KCI. 
O 

0.37IS 
0.7421 


kdc> 4 , 

2,0566 

1,8262 
I , 6306 


O 

0.4339 

0.8665 



Wt. of 100.9 cc. 
of Solution. 



101.47 
SOUJBXLITY OF POTASSIUM PxitCHLOMATV IN AQUKOUS SALT SOLUTIONS AT , 

Saturation was obtained by constant agitation, and approaching equilibrium 
from above and from below. The salt content of the solvents was determined by 
evaporation and drying the residw at 200. Thu salt content of the saturated 
solutions was determined in the same manner and the difference ascribed to dissolved 
perchlorate. 



Suit 

None ea 

KCI 


C.m, Equlv. Salt, 
perl (MM) fmn. II 8 0, 

HjO.. o.o 


ftm. Bqnlv. KCI 4 
pr 1000 frnt. 11(0. 

o.nSfj 

0.07,17 
o.o535 
0.1174 
o.ogjjC 

0,0(4'JS 
0.11*2% 
0.076% 

o.o >33 
0.1667 
o.iS58 

o, 173% 


CJ, Ijwl, Matt, (i 

Salt, jiwr lW,f ww, 11,0, j 

, IVaNOi ... 0.1008 
M ... o3 13<) 

K|2>(/4 H ,, o.oc^B 
>* .... o.3o%5 
> .... 0.6008 
Na t S0 4 . . . 0.1047 
... o.:^io 


;n>, Kqulv. KQ0 4 

iKr Kwo ftm. l^o. 

0.1790 
O.I09< 
0.II94 

0.0857 
0.0644 

O.l8oo 

0.1967 
0.1669 
o.i638 
0.1693 
o.i6o5 
0.1747 
0,1902 


i) 









KNO, 








w 


.... o 6686 


NaC10 4 






w 


0.627^ 


NaCL... 

n 


0.1007 


..... 0.599* 

BafNC)|) t . OIM^I> 
> , 0.3019 
M . 0.607 5 












791 KALIUM 

SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM PERMANGANATE AND 
POTASSIUM PERCHLORATE AT 7. 

(Muthmann and Kuntze, 1894; recalculated by Fock, 1897.) 



100 



Milligram Mols. per Liter. 


Cms. per Liter. 


men. iwr ecu 
KMnO.in 


r KMn0 4 . 


KC10 3 . 


KMn0 4 . 


KC10 4 . 


Crystals of So 
Phase. 


O 


63.91 


O 


8.86 


O 


29.37 


54.48 


4.65 


7-55 


2.84 


67.73 


42.75 


10.71 


5-93 


9.78 


79.04 


39-59 


12.50 


5-49 


10. 81 


99.8l 


38-63 


15.79 


5-36 


I5-96 


122.24 


34-39 


19-34 


4-77 


23.56 


119.21 


38.91 


18.84 


5-39 


24.28 


128.08 


33-77 


2O. 26 


4.68 


26.40 


I44-46 


33.14 


22.86 


4-59 


34-32 


167.81 


29-53 


26.55 


4.09 


44.42 


183.09 


25.19 


28.97 


3-49 


67-33 


197.82 


20. r6 


31-30 


2.80 


77-95 


233-75 


28.26 


36.98 


3-92 


94-37 


264.27 





41.81 





IOO 



EQUILIBRIUM IN THR SYSTEM COMPOSED OP POTASSIUM AND 
SODIUM PERCHLORATES AND NITRATBS AT 25 



0. Of 


Dms. per tOO 0ns. HO 


Solid 


sac. sol. 


' KC10 4 


IMaOOT 




^^ 




Phase 


1.013 
1.684 


2.07 


211.0 








KC10 4 
NaClO, 


H,0 


1.392 








91.7 





NaN0 3 4 




1.189 











38.3 


KNO* V 




1.684 
1.732 


0.87 


210.0 
209.0 


41-7 




KCIO. 
NaCi0 4 


+ NaC10 4 .K.O 
* NaNO 4 


1.512 
1.195 
1.733 


0.96 
1.91 


208.0 


97.7 
41.2 


49.2 
38.8 


KNO, + 
KCl5 4 


NaN0 3 

4- NaN^,, + NaCl0 4 .H p O 


1.419 


7.2t| 





94.4 


~ 


" 


* NaNO^ 


1.515 


1.92 





97.7 


49.1 


" 


+ " *- KNO^ 


1.070 


22. 1 











" 




1.758 




329.0 








NaClO. 




1-507 







175.1 





NaNO, 




1.569 
1.770 
1.825 


9.0 


333-0 
333.0 


114.0 


2/1 !: 


KNO, 
KCIO. 
NaClO, 


4- NaCXO. 
. -f NaNOj 


1.786 
1.609 
1.837 


22.0 
11.6 


331-0 


234.0 
116.0 


328.0 
255.0 


KNO, * 
KC10 4 


+ KNO^ 
4- NaNO, t NaClO^ 


1.578 


38.6 





186.0 





11 


4. 


1.803 


22.6 





242.0 


332.0 


" 


4 4- KNO a 



K KALIUM 7^)2 

SOLUBILITY or POT ASM xu* Pxnct*i.oitATit IN Awiou* ^ 

OF SODXim K'XTRATI AH6 VlC Vn*8A. 



<t of 
ant. 
sol. 



to*. pr 100 
pt. MI. aol. 



A>na 
HIM* 



tf of 

Ml* 

ad!, 



i^. ^r 100 
pit* MI. aoi. 



Results At o 



1.005 

1.136 

1.237 
1.317 
1.368 

1-352 



013 

.155 
.265 

419 

404 

1.392 



1.43 
1.70 

1.82 

1.88 
o.o 



0.0 
38*1 

36.8 



43.3 

Results at 3; 



a. 01 
2.25 
3-52 
3*6o 
3*S9 
1.82 
0.0 



0.0 

8.3 

40.4 

47.3 
47.8 



NaMO 



KC10 



Results ai 50* 



1.017 4.91 

1.158 6.10 

1*264 6.39 

1*349 6,33 

1.417 5.99 

1.468 5.73 

1.454 3.56 



0,0 

18*2 
30.6 

46.2 

51.0 

53.0 



KC10 4 






I.J13 



I. it SB 



,crt8 

. 170 

il 72 
515 

55 
.507 



10, Hi 

ia. j8 

v.6i 



. 11 



13, H 

i'ai 

5.17 



at 



41 7 
0.0 



1*1 
'11.5 



55.7 
56,0 



Icon.) 



57*1 

6l*7 



KCil) 



NaXO 



jH.17 o.o KOU) 



M 4> 

NaNO s 



or 



100 



aa.t* 
ol. 



Results 



1.005 0.75 0.0 

1.214 0*74 36.8 

1.309 0.0 26,4 

Resu lift at 25* 

1.013 2.03 00 

1.207 u6i 35.9 

1.198 o.o 36.6 

Results at 50 

1.017 4.71 0.0 KC10 

1*305 3.19 25*9 w * 

1.85 0.0 2fi.fi MM!i 



KCiO 

11 * 

NaCi 

KC10 4 

n^i 



4 f 

Ht. 



. 116 
.151 



6.18 
0.0 



.181 1*11 

ft A. i *. * 



1 100 
1W^ 

At t 

o.o wno 






IJI.7/ IV 



KCI0 



793 KALIUM K 

The following results are given by Cornec & Neumeister, 1929 for the 
(juar ternary system. 

KC10 4 + NaCl + NaN0 3 * H R 






d.of 


Ctas. per 


100 JU. 


sat. sol. 


Solid 




sat. sol. 


' KC10 4 


NaCl 


NaNO^ 


Phase 





1 342 


1.15 


16.4 


23.4 


KC10. T NaCl + NaNO_ 


25 


1 .404 


3-19 


4 1 


41.7 


' t NaNO, 


II 


1.395 


2.84 


8.4 


36.9 


n + n 





1.388 


2.55 


12.3 


32.5 


* " 4- NaCl 


II 


1-332 


2.31 


16.0 


23.4 


" + NaCl 


" 


1.274 


2.00 


20.5 


13-0 


" + " 


II 


1.378 


1.28 


12.8 


32.3 


" + NaNO, 


50 


1 445 


4.76 


8.6 


41.3 


KC10, + NaCl + NaNO, 

4 O 


11 


1.398 


4.60 


11.1 


34.6 


" t " 


11 


1.341 


4-34 


14.6 


25-7 


II 4. H 





1.277 


3.84 


19.6 


14*3 


H 4, 


75 


1.509 


7.69 


5.9 


48.3 


KC10 4- NaCl + NaNO, 

4 3 


" 


1.45M 


7.67 


8.1 


41-5 


n 4. H 


" 


1.384 


7-51 


11.7 


31-5 


H + H 


n 


1.305 


6.92 


17.1 


18.6 


It 4. II 


100 


1.578 


11.54 


2.20 


55-1 


KC10, + NaNO, 


II 


1.538 


5.86 


4-79 


55.5 


NaCl * 


' 


1.573 


10.80 


4.23 


53.6 


11 * " t KClO 


II 




11 .52 


5-73 


47.0 


4- KC10 4 


" 


1.440 


11.72 


8.84 


37-0 


II 4. H 


" 


1.340 


1 1 34 


14.71 


22.1 


H 4. '1 



SOLUBILITY OF POTASSIUM PJERCHLORATE IN AQUEOUS SOLUTIONS 
OF ETHYL ALCOHOL AT 44. 

(Pier rat, 1921.) 

Saturation was obtained by constant agitation for several hours. The saturated 
solution was evaporated to dryness in a current of air and the residue dissolved 
in enough water to yield the original volume of the solution. The salt content 
of this solution was then determined by electrolytic conductivity measurement. 

Wt. per cent (ons. K 01 O* per \Vl. pr emu (Jinx. KC10t per 

C 3 H & OII in solvent. liter sal. sol. CIfftOIl in solvent. liter sni. sol. 

o.o 12.4 4>..4 3.9 

7.1 9*^ 58.5 3.6 

1 3 . 2 7.8 94 . 7 o . 1 5 

27.3 5. 7 



SOLUBILITY OP POTASSIUM PSRCHLOIUTB IN AQUEOUS SOLUTIONS 
OF ETHYL ALCOHOL. 

(Flatt, 1933; Flatt and Jordan* 10 TO, 10^.) 

Vol. Percent fas. KC10 4 per Q Vol. Percent Obs. KC10 4 per 

in Solvent too jns. sat. sol. C jF * la Solvent too 0os. *t. sol. 



25 o (= H.,0) 2.065 'o 50 1./I22 

" 50 " 0.790 " 75 0.54S 

75 0.313 



KAIIUM 

lOOgms. 51.2 Vol. % Aq. CH*OH (d - 0.931*)) dissolve 0,754 Km JK1O at 25.2. 

oac " " (d -0.8219) " 0.051 gra*KCrO4 m a?25.2 Si ! 

70 O nm and Cumming, 1915.) 

11 0.019 gm. KClOi at 25.2. 

(Thin uml Cumming, xuiei 

, _ <* *vs**. ,.. tr/'-i/A /_- .o' 

90 

97.2 



, 

0,036 gm. KC1O< at 25.2*. 



, . 

0.0156 gm, KnO 4 at 25.2. 
(Wcnze, 1891.) 



SOLUBILITY OF POTASSIUM PBRCHLOHATK IN AQUEOUS AND IN ALCOHOLIC 

SOLUTIONS OF PERCMLOEIC ACID AT 25.2. 

(Thin wad Cumming. IM.) 
In Aq, HClOi Solutions. In Alcoholic HOO* SolutionH. 



Solvent. 



Normality of Aq. Gmi. KCia I 

HC10 4 . zoo Gmt. St. ad. .-.,. w , 

o (= water) 2.085 93-5% Alcohol 0.051 

0.01 x.999 " +o.2%HC10/ 0.0175 

10 1.485 98.8% Alcohol -|- " o.oxo 

1 0.527 " +a% HOC)/ 0,028 

* The HC!0 4 was added as aq. ao% HQ0 4 fotution hence th concentration <( the alcohol was decreased. 



OF POTASItH 



ABOU'TR ETMtL ALCOHOI, 



SOLUIIOH or AMNONXUM SALTS AT 



ol: 



Results for C^H^OH (d = 0,7852) 
Ammonium Nitraie Annonium 



ptr Uttr 



Iodide 



Holm er iittr 



^? 



0.000000 
0.000354 

0.000488 
0.000971 
0.001858 



o. 00056 5$ o.oooooo 

0.000506 0.00.0333 

0.0006311 0*0005 u 

0.0006773 0*001004 

0,0007a8l 0,001743 
0.0008396 



o 0003651 

0*0004970 0.000836 0.0006493 
000040ii7 UOOH4i 0,0006784 
O. OOI3k8 0*0007068 

0*0007156 

o. 0007462 



SOLUBILITY OF POTASSIUM Pencil ton ATE IN B 
(WitUnl n4 HmiUi, It. J 



fi 

Stulvrnt. sl * 

Water 

Ethyl alcohol 0.785* 

Methyl alcohol.. 0.7878 

n Fropyl alcohol o%8ou 



SOLVENTS AT 



it Butyl alcohol. . o.86o 



o. t*i 

o.oto Klliyl 



0.7868 



o.ooS 
o.i55 

0.(K)l5 



795 KALIUM K 

SOLUBILITY OF POTASSIUM PERCHLORATE IN NORMAL BUTYL ALCOHOL, ETC, 
AT 25 3. ( Smith, 1923 <r. ) 



Composition of solvent. 

...,., , - . _-^ Milligrams 

Per cent Pure Per cent Per cent KlO* per 
n Butyl alcohol. HCIO^H 8 0. H a O. 100 cc. sat. sol. 



Composition of solvent. 

, - ,.,!,.- - .. Milligrams 

Per cent Pure Percent Percent KC10 4 per 
n llutyl alcohol. IIC10 4 :iH 2 0. H S 0. JOO cc. sat. sol. 
IOO O.O O.O 1.35 

99.76 O.2D O.O I. GO 

99 . 5 o . 5 o.o i . oo 

99 . o i . o o o 1.9 

98.0 i.o i.o 1.4 

100 cc. pure ethyl acetate dissolve 1.3 mg. K Cl 4 at s5. (Smith, 1025.) 

SOLUBILITY OF POTASSIUM PERCHLORATE IN MIXTURES OF ETHYL ACETATE 
AND ALCOHOLS AT 25. (Smith, 1923.) 

Cms. ECU)* 
Composition of solvent. ir 100 gins. sal. sol. 



99-0 


0.0 


i .0 


2.0 


97.0 


O.O 


3.o 


3.8 


()6.o 


1 .0 


3.o 


1.6 


96.5 


0.5 


3.o 


1.2 


94-0 


i .0 


5.o 


2.3 



CH 3 OH o.3^ 



90 Vol. o/o CH 3 COOC,H,j 4- 10 Vol. 

85 4- i5 

80 > 4 2O 

90 )) 4- to 

85 4- i 5 

80 4- 20 

90 4-10 

85 4- 1 5 

80 4 2O 

90 -i- 10 

85 4-' 1 5 

80 )> 4- 20 ' 

SOLUBILITY OP POTASSIUM PERCHLORATB IN ANHYDROUS ACBTIC 
ACID SOLUTIONS OP VARIOUS SALTS AT 25. 

(Seward and Hanblet, 1933 Scholl and Hutchinaon and Chandlee, 1933.) 
Results for CH 3 COOH (d p? = 1.044) solutions of: 

Lithium Chloride Magnesium Chloride Ammonium Perchlorate 





o . 5 5 


C 2 H 5 OH 


o. i(> 









.. o.33 


of93/oC,H,()H ! 


.. 0.28 





.. 0.44 





. . o.So 


n Butyl alcohol.. 


.. 0.24 





. 20 





.. 0.2) 



Cta. Mols. per liter 



L1C1 
0.00000 

0.00070 
0.00141 
0.00285 
0.00641 
0.00943 
0.02870 



KC10 4 x 

0.000196 
0.000293 
0.000360 
0.000524 
0.000701 

0.000767 
0.001265 



Sodium Bromide 



Mols. per liter 



MgCl 2 

0.0000042 
O.O000115 
0.0000314 
O.OOOOi|20 
O.O000829 
0.0001440 

o . 0002820 

0-0005390 



da. MoXa x pr liter 



0.000228 
0.000250 
0.000276 
0.000297 
0.000336 
0.000347 
0.000394 
0.000475 



Sodium Bromide 



0.000198 


0.000194 


0.000316 


0.000176 


0,000378 


0.000190 


0.000509 


0.000171 


0.000765 


0.000155 


0.000983 


0,000155 


0.001306 


0,000139 


0.002093 


0.000141 



Sodium Nitrate 



Ghu 



.per liter 



0.000078 


0.000233 


O.OOOOO 


0.000195 


0. 00000 


0.000195 


0.000120 


0.000247 


0.000078 


0.000235 


0.000168 


0.000253 


0.000192 


0.000288 


0.000120 


0.000270 


0.000346 


0.000305 


0.000210 


0.000314 


0.000192 


0.000290 


0.000633 


0.000357 


0.000278 


0.000329 


0.000210 


0.000288 


0.001009 


0.000413 


0.000590 


0.000387 


0.000278 


0.000310 


0.001550 


0.000483 


0.000700 


0.000409 


0.000590 


0.000379 


0.001825 


0.000522 



KALIUM 796 

POTASSIUM OHEOMAT1S K s rO 4 K s Cra, KiCr t O lo , etc. 

EQUILIBRIUM IN THE SYSTEM, POTASSIUM OXIDE, CHROMIC ACID AND 
WATER AT SEVERAL TEMPERATURES. 

(Koppelaad BlumeathaJ, 1907.) 



Results at o. 

Cms. per xoo Gnu. Sul. 
Solution. 


Results at 30. 

GUM. per 100 Urns, Sat. 
Solutttm. 


Results at 60. 

Cm, j>er oo (*mi. Sat. 
Solution, 


^KaO. Cid. 


r kit). 


C*rt*4 KjO. C'f|t^. "^ 


3 1 


18 




. 


46. 


8 


alx>ut 50 


26 


06 


O 


54 


26. 


8Q 





Q4 


32 


,()B 


o 


53 


*9 


3I 


4 


.27 


22. 


25 


3 


06 


21 


.0 S 


9 


-*5 


17,06 


ii 


77 


x8. 


65 


1 3 


72 


2O 


2S 


14 


43 


17 


62 


18 


.71 


19, 


12 


20 


JO 


2O 


70 


ai 


,t>7 


17 


73 


19 


.04 


19. 


35 


21 




2O 


,6x 


23 


,61 


10 


90 


ii 


-93 


15, 


04 


x6 


HS 


14 


S3 


20 


.82 


I 


87 


3 


*$ 


XI. 


20 


1 1 


I! 


IO 


.ox 


21 


,21 


o 


78 


22 


-38 


2, 


4 2 


28 


21 


6 


.86 


39 


.64 




47 


42 


9S 


2, 


SO 


44 


5 


7 


.06 


4g 


,84 




,25 


44 


S^ 








, 


4 


,06 


54 


73 




17 


46 


.84 








. 


2 




60 


,69 




37 


47 


.40 


2. 


35 


49-95 




.24 


48 


23 


I , 


35 


S3 


39 













16 


56 


93 



















o 


64 


61 


79 


O. 


*6c> 


62 


81 


! 


,27 


S 


-77 


o 




6x 


54 






61 


S J 


O 






,12 



Temp, 



KtCrQ,* 



KtCrA, 



14 4-CiO, 
CfO, 

THE CRYOHYDRATBH (KI^TKCTU*H) IN TW SYSTEM K<() - Cr() - HiO. 

The points were determined by adding to a nut. notation of KtOtOr successive 
I to 2 gm. portions of chromic ark! *iml umwutninfc the frwxing-point and 
composition of the solution. At the* |H>int of nijifMw*trt<i r of *i new nolid phase an 
additional amount of chromic acid doe* not clung? th* f .-pt . Htm e the added Cr0 3 
goes into the solid Thin rtUtton atao hold* M tlw* point* where the flota- 

tion is simultaneously saturattd with KiCrM *AC| KiCrAi wr KsCrAi and 



t* of Equi- 
librium of 
Sat. Sol. 
with ice, 



CIM. pr 100 Cm*. 

S.lf Suits f ?! 






whh *itc. Sid, 

ami I. 
XgCiOi 



C*nti 



SMI 



.%tk! Fk% 
in KtjullibrlttW 
% withHftt.8ot 



f 



I4 

32, 

32 



-0*6j 
-1.78 
-5*5 
-6-43 
IO.2S 



,50 
,10 
It 

-26 77 

JO . JO 

-34 01 

-49 

-61.5 



not <U*t. 27,26 
28,85 

< JS^i 
36,14 

30.86 



20 s70' 

17-52 13.89 

17,12 18.18 

17.18 18,11 

8.27 8,oi 

x '3^ 2-93 
notdet 6.81 

11 16,05 
0.48 17,25 
0.45 23,63 

The viicosity of the oiutionii nt the lower trmperat urm incrraned o much that 
the cryohydratc could not be determined. By graphic extrapolation the 

cryohydrate tempemtwrt of chromic arid and of r ttrtittiic wid 4- potawium tetra- 
chrproate is w ^* and the CrOi if 59 per too sat. !utiou- 



o 47 

i,iH 

cis 

O-7Q 



4,1,31 

4J-4S 
4S^S 



not del. 49. xx 
o ox .$? 



797 



KALIUM 



By interpolation from the data given in the preceding tables the following 
solubilities in water are obtained : 

THE ICE CURVE AND SOLUBILITY OF POTASSIUM CHROMATE IN WATER. 

,o " Gms. K;tCrO< per Solid ** Gms. K 2 CrO 4 per o lid ph 

* ' 100 Gms. H 2 6: Phase. * ' 100 Gms. H 2 6. bolld Fhasc ' 



- 0.99 

1.2 

- 4.3 

7.12 
-10-35 

Potassium 
Bichromate 



-0.63* 
O 

30 
60 

104. 8f 



4.53 
6.12 
26.99 
42.04 
52.41 



per 100 Cms. 
H a O. 

4.50 

4.65 
18 . 13 
45.44 
108 . 2 



. 

Phase. 

Ice 11.35 EllteC. 

" O 

" 3 

60 
io5.8b.pt. 

Potassium Dichromate 
+ Potassium Chromate. 

r- ti A 

Gms. per 100 Gms. H 2 0. 



54-54 
57 -II 



Icc+KjCrO, 
K 2 CrO 



t - . 
-n- 5* 

O 

+30 

60 

io6.8f 



K 2 O. 

17.18 
17.73 

19.35 

20. 61 
24.3 



CrOj. 

i8.ii 
19.03 

21 

23.61 
30.5 



74.60 
88.8 

Potassium Dichromate 
+ Potassium Trichromate. 

Gms. per too Gms. Sat 
4^ Solution. 



* Eutec. 

Potassium Trichromate + Potassium 
Tetrachromate. 

Gms. per 100 Gms. Sat. Sol. 



-30- 

o 

+ 20 

30 
60 

H4t 



K 2 0. 

1.18 


Cr0 3 . 
42.51 


1.47 


42.99 


2. 2O 


43.10 


2.50 
7,06 

16.80 


44-5 
49.84 
59.20 



t b. pt. 

Potassium Tetrachromate + 
Chromic Acid (Cr0 3 ). 

Gms. per i oo Gms. Sat. Sol. 



If . 


K 2 0. 


Cr0 3 . ' 


39 Eutec. 


0.79 


45^9 


o 


1 .37 


47.40 


20 


2 


48.46 


30 


2.25 


49-95 


60 


5.01 


54-09 



o 

20 

30 
60 



JC 2 0. 

0.64 

O.62 

0.69 

1.27 



CK) 3 . 
61.79 
62.80 
62.81 



"Data for boiling points in the system KaO + CrOa.HaO determined by means 
of the Beckmann apparatus, are also given. 

The older data for K2Cr04 and K^CTrgOr are as follows: 

SOLUBILITY OF EACH IN WATER. 

(Alluarrl. 1864; Nordcnskjold and Lindstrom, 1869; Etard, 1894; Kremers, 1854; Tilden and Shen- 
stonc, 1884.) _ _ 

~" Potassium Dichromate. 



Potassium Chromate. 
Grams per TOO Grams Watqr. 



Grams per zoo Grams Water. 



O 


58.2* 


59 -3t 


60. 2 1 


10 


60.0 


61 .2 


62.5 


20 


61.7 


63.2 


64-5 


25 


62.5 


64.2 


64-5 


30 


63-4 


65.2 


66..S 


40 


65.2 


67.0 


68.6 


50 


66.8 


69.0 


70.6 


60 


68.6 


71.0 


72.7 


70 


7o-4 


73-o 


74-8 


80 


72.1 


75-o 


76.9 


90 


73-9 


77.0 


79.0 


100 


75-6 


79.0 


82.2 


I2 5 


79.0 






Z 5. 


83.0 







* Etard. 



t Alluard. 



N. and I*. 



5* 


5 


7 


7 


12 


12 


16 


16 


20 


2O 


26 


27 


34 


37 


43 


47 


52 


5* 


61 


70 


70 


82 


80 


97 


no 


145 


143 


205 


A., K., T. 


undS. 



K KALIUM 

SOLUBILITY OP POTASSIUM CHROMATICS IN WATER AT 30. 

(Schrrincmtker Z, phyiuk- Ch. 55 *J. '06. ) 

Composition Wt per crftl <l: 

^-^------- ---~---*-"*- " """'"" *-.'' --' ,.,.,.. ,,.-..,,,,,^, *.>>...- ^ Siiiitf 

The Salmi m Thr Rridur. , 

Per cent CrOt I'cr ceal K*O . IVrrcratttOj. rrcat Kt>. 



O 


47 






o.o 


47.16 


12.59 


47-54 


0*1775 


34.602 


10,93 


37 -47 




26.602 


16,482 


3* '53* 


5.598 


20.584 


37 -*3* 


3<M;a2 


15.407 


19.325 


27.966 


*9'377 


20.67 


19.17 






19.096 


17,30 


37,64 


22,61 


".35 


7,88 






17-93 


3,412 


25 .85 


7 -8a 


43 -S* 


3.01 


49,45 


9-9* 


44.46 


3 -245 


S3 -94 


la 40 


46.368 




60.314 


93S 


49-357 


2-3$3 


63.044 


11,684 


53-215 


1.360 


63,95!! 




62.55 


0,796 


67.944 


6,731 


62.997 


0.621 


70-0 


4-0 


62.28 


oo 







CrO 

ioogm.8at.>luiitinmglyctil,rfH(<)H)i.Ht() l cofiM*n 1.7 Kim, Kit V()at 15,4. 

IOO gms. sat, nolution in glycoi, Cil I*(OI I h. 1 ItC I, amuin 6 gmM. Kit T A at 14,6. 

(<lr trmck, 1905.) 

ioo gms. H|0 disiolvc to.i guni, KttVA at 15.$ (t*ni*h ami Smith, tpi.) 



100 gms, sat, solution in water cnntntn 5.5* KfC>fC> t at 4,81 " 15,17 gms, 

at 30.1 and 17.77 at ^S-33*' , f % lf '** tlliflf * wl **miKii, 19110 

ioo cc. sat. tqueou iclution contain 1 1.43 ntn*i, Kit*rit)i ii ao*. 

(Stwrritt a4 Eaton, 1907.) 



SOLUIIUTY or roTAH*tm CMI^ATIS IM 

lfliliWi Wff! 

lor ttf*^tilt*t fur Fni^iliiw 01 C 



. 

1 tic, ael* WO pi* MU wt. i. i*l* IOC *>* i*i. wi. 

IS l3749 38<I9 1* lol*1* 8.893 

20 1.3785 38.94 J i.wAH 10. Baa 

sis 1.3805 30-18 J>, t,f* lH 12.98 

The following ort r<*cffiii rt**i4*rwtii.tiioii of ih^ 5kilti&liii| of Potassium 

DlChrOfiate in W^ttr are given iy t.ikiwilt AWI! 



Gws. KCr0 per 100 



7QQ KALSUM K 

SOLUBILITY op POTASSIUM CHROMATB IN WATBR 

AT TEMPERATURES ABOVE 100. 
(Benrath, qjedebo. Schlffers and Vtaiderllch, 1957.) 

The authors' results were plotted and the following values taken. from 
the average curve. 

Ctas. K 2 Cr0 4 per 
c 100 ena. sac. aol. L 100 Ss. sac. sol. 100 eps. MC. sol 

100 4/4-. 180 48.5 2*0 52.6 

120 45.5 200 49-6 280 53.6 

140 46.5 220 50.6 300 $4.6 

160 478 240 $1.6 320 55-7 

SOLUBILITY OF POTASSIUM CHPOMATB IN AQUEOUS SOLUTIONS 
OP SEVERAL SALTS EACH DETERMINED SEPARATELY AT 25. 

(Herz and Hiebenthal, 19?9.) 

Results for Aqueous Solutions of: 

Potassium Potassium Magnesium Sodium Ammonium 
Bromide Chloride Chloride Chloride Chloride 

Oto. Mol. j?er ll ter Qa. MoL j?er liter Ota. MO L per liter (ta. Mol. per liter On. Mol. per HUT 
^liF i/e Kcro x lea i/* KCro '1/2 - A ~" A 



0.00 


8.35 


0.0 


8.35 


0.0 


8.35 





.42 


8. 


22 0. 


45 


7.68 


0.41 


7.56 


0.40 


7.76 


0.42 


7.58 





.86 


7. 


71 0. 


83 


6, 92 


0.82 


6.91 


0.46 


7.69 


0.86 


6.11 


1 


73 


6. 


51 l. 


81 


5^58 


1.24 


6.26 


1.31 


6.48 


1.73 


4.30 


2 


.59 


$ 


46 2. 


34 


5 . ou 


1.78 


5.50 


1.72 


5-89 


2.27 


2.74 


3 


-30 


4. 


79 2. 


93 


a.n 


2.19 


5.00 


2.18 


524 


2.76 


1.30 


3 


.4-0 


4. 


$7 3. 


76 


3*'J9 


2.70 


4-38 


+2.70 


475 


3.26 


1.04 


+4 


2$ 


4. 


no 4. 


SI 


2.87 



Cr 



SOLUBILITY OF POTASSIUM CHROMATE IN AQUEOUS SOLUTIONS OF POTASSIUM 
MOLYBDATE AT 25 AND VlCE VERSA. 

(Amadori, 191 aa.) 

Cms, per TOO Cms. H 2 0. Gms. per 100 Gms. H 2 0. Cms, per iqo Cms. HjO. 

" " 



K 2 CrO<. 


KMo0 4 . 


K 2 CrO 4 . 


K 2 Mo0 4 . 


64.62 


O 


J4-I3 


98.72 


49-59 


15-37 


10.07 


II8.8 


38.90 


38.79 


10.24 


II9.9 


33-21 


50.96 


7.12 


137.8 






6-37 


157.2 



4.92 165.4 

2.14 180.8 

1.70 183 

o 184.6 



SOLUBILITY OF POTASSIUM CHROMATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM SULFATE AT 25 AND VICE VERSA. 

(Amadori, 191 aa.) 

Gms. per 100 Gms. H 2 0. Gms. per 100 Gms. H 2 0. Gms. P$^g^9'jj[ 

K 2 S0 4 . ' 'K 2 CV0 4 , " " 



63.09 0.76 40.93 3.33 7.81 8.<)8 

61.39 I.I7 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 O 12.10 

ioo cc. anhydrous hydrazinc dissolve I gm. K 2 Cr04 at room temp. ) (Wehhand Brod- 
100 cc. anhydrous hydrazine dissolve I gm. KgCraO? at room temp. J erson, 1915.) 



K KALIUM 

SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM SULFATE AND POTASSIUM 
CHROUATK AT 25* 

(Fock. ; 



MUlkram 


MoN. per Liter* J^SSLSLlJlSLL^. 


MM!, ftf 


r ,T n nl *> Cr - *$:&** 


"KaR0 4 . 
6I.8.I 
608.4 
341.0 

174. a 

110.7 

IOO. 6 


O 

103 

691 
1496 

2$^3 
2687 


rO*. 
.O 

.8 
o 


KjSU,. 

1077 

106,0 
59.46 
30.47 


o 

30 
134 

4<p 


,00 
02 

5 

5 


100 

10 

4 

J 


itn. ! 

O 

50 

<>o 


Mtltttirun, 
OO^ 

.141 

377 


IOO 

99 
97 

gi 

28 


|in 

UM. 

O 
.6 S 

'30 

97 

43 


o.o 


2847 




O 


O 


553 


S 


a 


a> 


308 





-00 


734-o 





.0 


127 


9 





o 


IOO 


o* 


.oi63 


100,0 


617.0 


103 


4 


107 


6 


20 


i 


% 


^S 


0034 


99 


.78 


4^3 


452 


-7 


80 


72 


HK 


o 


55 


SS 


**3S 


98 




279 


948 


.2 


48 


64 


184 


4 


23 


72 


.17^ 


96 


.07 


IS3 


1469 




36 


.68 


*S 


.6 


9 


41 


32^ 






296 


2681 




5* 


,61 


5 


.2 


21 


og 




25 


73 


o.o 


2715 







,00 


5*7 


.S 


O 


00 


,3781 


o 


00 



THE SYSTEM AMMONIUM (*tituMAii; f l*tirA*i 

lArki v t t 
(iins, j>f tt>0 |fHi, < 

Ml, 4>U 

KOrO^. (Mi.iftCt'Ot' Hiiii*! Mt#*#* k t ' 

39.35 0,00 

36.77 < 

34.38 1.i5 _ . 4-V 



f WATH AT 



ii*iM 



10.01 



of 



Serif* 



l8.6.< tS*5 
16.07 *9* J 
i5.8< 19.9 

A STUDY oy TIW 



n 



4.t4 

I t . lk| 
7.118 

4.'il 



14. HH 

7 1 , i i 



Mixiun^s 

of th two series 
of ottd tolutioos 

Series 
of ftoitde solutions 

of KfCrOi 
in(NH*),CrO* 



I*AW KHIIJ,. K 1 !C:r< 



Previous exporimonln Utvr ihtmii thut K A SC.) $ t K s Cir > 4 4m! !* (NHJj S0 4 -f 
K| S0 4 ftach form eomptot* of o)t4 oiutton* with n |tt|i f wlti!(N H|] ft Cr 4 -j- 

(NH 4 } t S0 4 and (NIIJi Cr U 4 i- K f Cr O oH ftirw n^riri if nottci aoluttoni with 
gaptreipictivolyti.90toii,5i ttitl rft^S to 55. So ittwbr ft*rrrtttAjt<t of ammonittm 
chromate. Thd prwent nxpmmrtiti wtr0 ly iiliiig to otution in equili- 

brium with two kmdi of iiilldl notation* *f two liftvitig * rommon ion another 

salt in diffftititt proportion, in mit'lt * ntftiitwr ttmt whru r>c|iiiiibrtttm is attained, 
two or thrw solid rcmat 111*1! ti rmitihtr. Ilir mixture* wr rotated in a 

thermoitmt for at two day*. Tho of tin* iini given in a table 

and plotted in the Janwcke diagram. 



AMMORXini Unthanmn 

Data showing thai tltr f of tin* Uoubfa ammitmum ianthanwn 

chromate if in the of oiutton rontasttiitg from 5.o6 to 

per cunt of amm0niii chromate, art by Cambbt, f yt> 



8oi 



KALIUM K 



POTASSIUM DiCHKOMATE K 2 Cr 2 7 . 

SOLUBILITY OF POTASSIUM BICHROMATE IN AQUEOUS SOLUTIONS 

OF SODIUM DlCHROMATE AND VlCE VERSA. (Robertson, 1924.) 

The mixtures of the two salts were dissolved in water at a higher temperature 
than that of the isotherm and the flasks then placed in a thermostat at the desired 
temperature. Constant agitation is not mentioned. 



Results at 25".. 

,. sol. 



Results at 50. 

Gins, per 100 pins. sat. sol. 



Results at 100. 

Gins, per 100 gms. sat. sol. 



jms. per auu 

<- . - 


glll. d.l. BUI. 

**" *- 


vxmtt. per juv 

-^^ 


gm. an. nvi. 

s - 


\*ma. ins* ivu 

*-"" ***... < 


' giua. .-><. jwi. 

" **- -* 


Solid Mmsr 


Na a Cr a 7 . 


K.Cr.O;. 


NajOjOT. 


K,Cr s 7 . 


>"a,Or s O T . 


K s Cr a 7 . 


at each tompenUuro. 


O.O 


l3.I 


O.O 


27.4 


O.O 


47-^ 


K 2 r 2 7 


4.38 


12.2 


6.5 


24.2 


6.3 


42.1 





16.1 


8.68 


i6.3 


19-3 


14.1 


36.5 





20. o 


8.97 


21. 


17-8 


23.0 


a9.o 





26.9 


7.70 


29.3 


1 3. 6 


29,6 


24 . 2 





33.6 


6.5?. 


43.6 


n. 3 


44.4 


16.4 





43.2 


5.46 


48.5 


9-47 


56.r 


i3.4 





55.5 


5.i6 


52.5 


9.36 


60.6 


12.4 





61.4 


5.25 


63.3 


7.92 


70.8 


9.96 


Ntt.C^O; 


65.5 


O.O 


70.3 


O.O 


80. i 


o.o 


Na s (:r s O 7 



SOLUBILITY OF POTASSIUM BICHROMATE IN AQUEOUS SOLUTIONS 
OF POTASSIUM CHLORIDE AND VICE VERSA. (Robertson, ifl^,) 



Results at 55. 



Resulls at 50. Results at 100. 



Gins, per 100 gms. 


Gms. per loo gm$. 


Cms. per JOO gms. 


sat. sol. 


sat. 


sol. 


nut. 


sol. 


- *-^*> 


**~**~ 


*~ ***->' 


^^00^ --, 


* -*-_ 


s*^***--^ Solid IMinsn 


KC1. 


K.Or.O,. 


KCI. 


K,Cr a 7 . 


KCI. 


K s Ci' a 7 . nl each tempernt'irc 1 . 


2.1 


IO.O 


2.4 


25.8 


O.O 


47-2 KjCr^Oy 


4.3 


8.3 


4.6 


21.3 


3.5 


42 . I 


6 32 


6.53 


6.6 


l8.() 


7.2 


37 . 1 > 


8.2 


5.5 


8.6 


I6. 7 


u.4 


32.2 


10. 


4.55 


10.6 


14-9 


i5.6 


27 . 6 n 


1 1. 6 


3. 9 


11.9 


J3.2 


22. I 


20.6 


i3.o 


3.36 


i3.3 


12.4 


24.9 


18.2 


15.7 


2.6 


14.8 


It 




n 


18.6 


2 . 2 


18. i 


8.8 







21 .2 


'7 


21.4 


6.8 







23.0 


1.5 7 


24 . o 


5. 7 




> 


26.0 


1.2 


28.9 


4 . i 


27.6 


1 6. 2 4-KCI 


- 


- 


29 . o 


3. 7 


29. () 


n. 6 KCI 


26.1 


r.o5 


29.8 


1.9 


31.9 


6.4 


26.3 


. 


3o.6 


0.0 


35.9 


o.o 



Cr( 



KALIUM 

POTASSIUM 



Bo 2 



SOLUBILITT OF POTASSIUM Dies ROM ATI is Awxong SOLUTIONS 
OF SEVERAL SAWS, BACH DKTIRNXWID SSPA*ATXLY AT j s a . 

fBft a Hltbtnihtl* tiff.) 



Results for Aqueous Solutions of; 
Calcium Chloride Magnesium Chloride 



Molt, ptr littr 



0*24 
0-4S 



1.64 
1.87 



2.88 

2.84 
3*69 
2.62 
3.56 
1.88 



Lithium Chloride 



ptr Uur 



0.0 
0.45 
o * 9 3 
1.89 



a.Hg 



1.7& 



Strontium Chloride 



Hail, ptr ii tr 

" 



0.0 



I , oo 

Jt.03 



3,89 
3*Bo 
4.91 
2.7.) 

2*69 
j.6a 



Ammtmium Cli 



CrO 



Holt, ptr 



Holt. er littr 



TEST 


t/ryr ? 7 




w-V f VV 


WH/i 


W"V p f! 


0.0 


2.89 


O.U7 


3. Ml 


o.o 


2,89 


0.49 


3.73 


0.94 


3 >H 


0.71 


a.Sa 


0.92 


a, 55 


1.91 


a. 79 


I* 79 


Ji'Sii 


1.78 


a.aS 


3.8*$ 


J.fej 


J * 59 


3t w 


2.78 


1*85 


3.80 


a. i! 


l.Ifl 


a. 16 


3.61 


1.S7 


4.31 


-i. jti 


14 . Pii 


1.83 


4.49 


1,33 


$03 


4 . 06 


$ IJ 


0,91 



POTASSIUM 



DlCRTOHATS If Sotlif df Dlft|A$H AT 

iMtrt ano 



Results for: 



ftttAHtittfll 



Oft. HOit. 



iittr 



* 



iittr 

, Mi* 



5-0 

9-0 
55. 
So 



1.31 

1.08 L 

0.0s U 

0,03 



10 

! '.$ 

5tl 
6 1* 



L 5 Lower liquid layer 11 = Ii.|it4 



o. js 

e. 15 

0.01 



803 KAllfJM K 

SOLUBILITY OF POTASSIHM CHROMATS IN AQUEOUS 
SOLUTIONS OF URETHAN AT 25 

(Pal I tsch, 1928, 1920,) 

On. Mols. per^tOOQ gns. H g O Solid 

KCr0 NKCOOCH. v Phase 



3.323 O.O KpUru^. 

o.i 49.61 Upper liquid layer 

3.0 0.396 Lower liquid layer 

Fusion-point Data are given for the following mixtures. 

K CrO + K Or 0, (Groschuff, 1908.) K 2 Cr 27 * K a M 27 ( Amadori > ion.) 

4 K MoO (Amadori, 1913.) " * ^W 7 

4- K WO " " " + Na Cr 2 7 (lehrman, Soldi tch 

* K S0 4 ( " ' Groschuff, 1908.) and Skell , 1936.) 

POTASSIUM FLUORIDE KF.2H g O 

SOLUBILITY OF POTASSIUM PUIORIDK IN WATER. 

(Jatlov and Poljakova, IOTP.) 

Qtas. KF ptr Solid Qroa. KF per tfolld 

c 100 BBS. sac. sol. Phase c 100 9n. eat. sol. Phaet 

-3.2 5.0 Ice 20 48.70 KT.?.H p () 

-6.5 10.0 " 25 $0.41 " 

-12.2 15.0 " 30 51.95 " 

-19.5 20.0 " 35 S4.65 

-2i.8Eutec.2i.$ " * KF.^H^O 40.2tr.pt .58.08 

-20.0 22.7 KF.4H ? " o 44.30* 

o 30.90 " " 17.5 47-52* 

10 34.87 " 4$ 58.62 

15 38.13 " 60 58. 72 

17.5 41.52 " 80 60.01 " 

17.7 47.7 " + KP.aH p O 

* Met ast able 

100 gms. sat. solution of Potassium Fluoride in Water contain 48.0 
gms. KF at 18 and the Sp. Gr. of the solution = 1.502. (Mylius and 
Funk, 1897.) 

Determinations by Forcrand, 1911, at 18 gave 45.3 gws. KF per 100 
gms. aqueous solution in contact with KF.2HJ) as solid phase and 33.96 
gms. KF per 100 gms. aq. solutions sat. with KP.nH^O as solid ph&s^. 

SOLUBILITY OF POTASSIUM FLUORIDE INT HYDROFLUORIC' Arm AT 21. 

(Ditte, x8t>C.) 
Gms. per too Gms. HgO. Gms. per^ioojQnniB. HgO. Gms, per TOO Cms. HfO. 

o.o 96.3 

I. 21 72.0 
I .6l 6l .O 

3-73 40.4 

4-03 32.5 
6.05 30.4 

loocc sat. solution of Potassium Fluoride in liquid hydrofluoric 
acid contain 38.0 gms. KP at o. (Fredenhagen 1930, 1933; 
and Cadenback, 1931.) 



' HF. 


KF. 


HF. 


KF. 


9-25 


29-9 


20.68 


38,4 


11.36 


29.6 


28.60 


46.9 


12 .50 


30-5 


41 .98 


61 .8 


13-95 


3*-4 


S3-7* 


74,8 


15.98 


33-4 


74-20 


1O5 ,Q 


17-69 


35.62 


119.20 


169.5 



K KALIUM 

POTASSIUM FUIOHIDB 



hoif 



FRERZrNG-POtNTS Of MIXTURES OF POTASH?H pLtmtlM AHP HYDROFLUORIC ACID. 

ffMf* 193O 

A thermocouple thermometer was us*tt Anl the freezing, eutectic and 
transition points were determined by coolUfi curves. Oat A for vapor 
pressure are also given. 





Hoi. Fraction 


tj 


t 


KF la Solution 


p 


-83.7 


1.000 


HP' 


-85.2 


0.987S 


M 


-86.9 


0.9712 


M 


-89.$ 


Q.9$8Q 


M 


-92.8 


0.9466 


M 


-97.0 


0.93" 
0.9143 


" + 

KF.nllF 


8^0 


0.8884 


H 


48.0 


0.8572 


H 


61.2 


0.8155 


t 


67.7 


0.8341 


M 


71.8 


0.8086 





(72.0) 


6. 8000 1 


M 


72.0 


0.7993 


** 


71.0 


0.7901 


tt 


67.8 


0.7783 


W 


(63.6) 


(0.771 ) 


ti 4. 


64.4 


0.7676 


KMHP 


65.4 


0.7583 


N 


(65.8) 


(0*75001 


It 


65.8 


0*7490 


M 


65.$ 


0.7438 


tt 


64.5 


0.7342 


*t 


62.6 


0.7278 


t* 


62.4 


(0.727* 


* 


62.7 


0.735 


KF.5HF 



70. o 

71.7 
71.1 
AS. | 
84. 
taH 



JI7 



Hoi. ffftctton 
r in Hdiution 



aoiid 



(t.7171 KP.slIP 
1 0.7111 1 fl 

0.71 is ** 

0.70410 " 



0,6777 



en 60 in 



KP.aHP 



a KF.HF 



w t tf KP.HP 
0.5418 ft KP.HP 

0.5101 
0.5075 ^ 

(0.5000) w 

0*4t99^ W 



If 



Acid PLUAKXDI KHP, 

nr PoTAasniH Ac 10 i?yf>ii in WATER. 






-2.9 
-4.9 
-7.6 


+10 



tOQ pi. wiu 

5*0 
100 

16.5 
33*14 



Ice 



KHP 



30 

5 
KKK, 60 

m 



NO I. 



53-38 



805 KAL1UM K 

POTASSIUM FLUORIDE KF 

SOLUBILITY op POTASSIUM FLUORIDE IN PURE METHYL ALCOHOL 
AND IN PTTRB ETHYL ALCOHOL- 

(0muth f 1931.) 

Results for Methyl Alcohol Results for Ethyl Alcohol 



t 


Gtos. KF per 
100 0H8. sat. sol. 


L 


(ins. KF pel 
100 . at. 


20 
30 
40 


0.192 

o. 168 

0.150 


20 
30 
40 


0.106 
O.096 
0.068 


50 
55 


0.12$ 
0.092 


50 
5S 


0.021 
0,0l6 



100 gnus, liquid Sulfur Dioxide dissolve 0.018 gro. KF at o- (Jander 
and Vickert, 1936; Jander & Ruppolt, 1937.) 

1000 gms. pure acetone dissolve 0.00022 g^s. KF at 18 and 0.00025 
gm. at 37, as determined by specific conductivity. (Lannung, 1932.) 



EQUILIBRIUM IN THE SYSTEM POTASSIUM FLUORIDE, ETHYL ALCOHOL AND 
WATER AT 23-26. 

(Frankforter and Frary, 1913,) 

The authors determined the binodal curve, the quadruple points and two tie lines. 

Gms. per 100 Cms. Upper Layer. Cms. ptr too Cms. Lower I, aver. 



KF. 


C 2 H 8 OH. 


H 2 0. 


KF. 


CH, ( CW. 


HjO? 


1.23 


92.67 


6.07* 


45.33 


0,67 


54* 








37.82 


1 , 70 


60 , 4> 


l!l6 


33.30 


15-54 














28! 68 


4- 7 


66! 8$ 


2.S6 


65*81 


31-33 








4.47 


57-4 


38.13 


20.90 


11.9 


67! af 


5-47 


53-04 


41.49 




. . 




... 






isiss 


% S .6 


65! 85 


6-93 


47.52 


45-55 








8.84 


41.28 


49-38 


*5'7 


ai!s 


6i!st 


9-55 


38.66 


5^-79 














13.57 


27.27 


50-15 


10.52 


35-91 


53-57 














"43 


33 23 


54 34 


ii 


30 


59 


II 


30 


SQt 




* Quad, points. 


t Tie line. 


t 


Plait point appmx. 





A method for the determination of alcohol in unknown mixtures, baned upon the 
above data, is described by the authors. 



F 



K KALIUM 5cl5 

THE BINQD\L CURVE FOR THE SYSTEM !*or.\ssn' FU?ORH>K, Pxora, ALCOHOL 
ANI> WATUR AT ^v'-J< 

iSKr.ittMttfltf attol i'fin. * I * 
Cms. per looGms, Hointwtu-tnrt Ufii*i, (i '* !*V' >J *'"''* *J' >in "* i n< liquid, 

.................... "~" " ' " ~ 



, " ro K i-' < MM w " 5r 

96.78 ^ *\S* H ! S 7 4Q 84,36 

1 78.91 -M 1C) 10 5 t)7 84,03 
0*62 66,29 .M <X) Jl 4 30 83.4! 
o.Si 50-97 .W *' *4.H 3 45 82.37 

j 20 47.40 NI it i** ;> t Ht) 7Q , 3S 

I<77 35,40 fJ H| .S Hi 0,74 73, 43 

2 50 IC),05 ?H 4\ J> ^ O -\$ 64,38 
5^32 10.64 4 04 41 *>* 0.030 5^.34* 



One tie line was cletermifiwi In f his f,t^* th<* iififwr liyrr ctmtuinwt 
CiHrOH and 0,31% KF, and thr litwor l.tvi't aiiLitiiril t>.c7' ;, KF, 

In this system, the* HlVti of t'li*tKr in t4iftfrf4?ttfr is ion* uuirketi them in 
the preceding one in wlurh ethyl *tirhti! in |iir^;tii 

100 gnm sat. solution of {.lotaHsiutn rtu>iU* in t)*).f r j. pr*>jyl alcohol contain 
0,34 gm. KF at r>m ttrmp. (KrAnkfrirr ami Fruiy, 1913.) 

BINODAL CURVE FOE THE SVSTKM PorAHMitM F!,ru!iiK !sti*RopYi. ALCOHOL 
ANI> W.XTHR AT Jf>". 

(KrAnkfmtrr Ami l'rm|lr, 1^11 ) 

Results in terms of gmn. fM*r nx of solvent, iilrnlitil -f w*ifer, 

Cms, per 100 (Snw. Slvrni <* lf f Solvent, 



51,826 ' 1,555 OH 445 ** 3 H $ Ji 4,jK 7^,562 

38.748 2.965 9? 035 5 oyt 50 .UO 40.661 

26.03Q 6.525 t)j 475 3 071 '$ 4$S ,14-545 

17.812 0, HS 1.705 Ha, 750 17*350 



BINODAL CURVK FOR ttiic S^nai INUANMI'M ri,t 4 iwiiH^ Att.vt, AI.COHOI* 
,\NI* WAI hi \r ^*>'. 



ir, t 



The rcHultH art* given in terniN f gratttH |'i IK g 1 "'- \l'bl !- Water instead 
of gnm, per I<K> gnw. <il the lutttKiKeneot 



ii*i % M i iiji inii 5 iii if-c)^ 

45.707 i =^70 t)7 7P 7 *t>S fs |ijt> 04 6to 

38,076 ,|.*Al i|Cit; 6 i) *,$ |j on S?- 1 ^ 

30,675 v s fyft) i|| I.M 4 Ki i 47 ^o 5^ 4S 

24,341 7,. i at) <)j., X|i t fMi vi Jit 4$'7&> 

20,580 q,6()i cp 401) ^ J 16 vi )4H 3^443 

17,371 11.491 l tip IH C>|0 34*37 

13,184 17,764 Mi.ijCi I 6H ^ %1 P' X SS 

10,880 21-5,17 77-4^3 ! i e> ^ 7 1 W^ 38,605 

8,873 29-5^0 70-47 i *'< f * 7S <77 ^4-^i 



807 KALIUM K 

BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, ACETONE, WATER 



AT 20 

(Frankforter and Cohen, 1914.) 



Gms. per 100 Gms. Homogeneous Mixture. Gms. per 100 Gms. Homogeneous Mixture. 



' KF 


(CHahCO. 


HA 


' KF. 


(CHjJaCO. 


HA 


46.3 


trace 


53-7* 


9.17 


23-53 


67.30 


44-24 

33-34 


0.24 
i 


55-52 
65-66 


3-06 


38.72 
47-89 


56.28 
46.84 


29.86 


i. 60 


68.54 


1.38 


58.06 


40.55 


25-74 


3.02 


71.24 


0-979 


62.60 


36.42 


20.28 


5.90 


73.80 


0-75 


65.41 


33.84 


16.31 


9.72 


73-97 


0.50 


69.58 


29.92 


12.40 


15-59 


72.01 


o 


98 


2* 






* Quad. 


point. 







Data for 4 tie lines are also given and the approximate position of the plait 
point is shown on the diagram. 

Several points on the binodal curves at temperatures between o and 35 are 
also given. 

A discussion, with examples, is given of the applicability of the above data to 
the determination of acetone in unknown mixtures. 

BINODAL CURVE FOR THE SYSTEM POTASSIUM FLUORIDE, METHYL ETHYL 
KETONE AND WATER AT 20. 

(Frankforter and Cohen, 1916.) 
Gms. per 100 Gms. Homogeneous Mixture. Grns. per too Gms. Homogeneous Mixture. 



KF. 


CHa-CO.CaHj. 


HA " 


KF. 


CHu.CO.QH*. 


HA 


34.38 


0.17 


65.45 


10.50 


4-87 


84.63 


23-63 


0.50 


75-87 


5-70 


9-93 


84.37 


18.62 


1.49 


79-89 




12.42 


83.61 


15.91 


2.19 


81.90 


0.84 


21.23 


77-93 


13.80 


2.98 


83.22 


0-34 


23-55 


76. II 



SOLUBILITY OF POTASSIUM FLUORIDE m IQUBOUS SOUJTIOHS 
OF I so PHOPYL ALCOHOL AT 25. 

(Qlnninga and Chen, lost.) 

The results locate the binodal curve of the system, including 4 lie 
line, *, which shows the composition of two liquid layers in contact 
with each other and, the plait, PP, at which the two liquid 
become homogeneous. 

fas. per too 0ia. eat. aol. QBS. per 100 ipm, tint* 



0.16 46.75 23.40 6.ao 

2.20 25.00 36.80 4. '\ PP 

445 l8.68 39.20 4*0 

7.70 14.30 65*80 x.o * 

1510 9.30 



K KALIUM 



808 



SOLUBILITY OF POTASSIUM FL0IIH IM AQUItOt!8 SOLUTIONS OF 

TERTIARY B*?TYL ALCOHOL AT -jo. 

and to&uint, i$no.) 



The points on the bi nodal curv of this :*y*t*m were di't^nnined by 
observing the appearance or di sappMr-xnce of cikidni^ in * mixture* of 
weighed amounts of KF and one of T|I* liquids, upon addition of a. weighed 
amount of the other. Conjugate points repr***nnh|i the iin* * legated 
by determining KP in two liquid layers in eoui-tct with each other, The 
plait point, PP, was found by plotting. 



Ctas. ptr 100 jpi. a 


uiu ol. 


ffca* pur 100 Jiiii 
__^..-N,^ 


'Uiv ; . -Mn, 








\ 3 ; 3 




3 3 




0.2 


51*9 


8,3 


10,1) 


0.7 


39*8* 


a. 7 


9.6 


1.2 


34.6 


9*7 


ft. 8 


1.6 


22.3 


xa.s 


7.0 


1.9 


20.7 


U*9 


u? 


2.4 


19.7 


IS4 


* ,f 


2.8 


18.7 


16.6 


5.1 


3.8 


l6.9 


17. 7 


^.5^ 


5.6 


lc|.0 


" 


i. \* 


6.1 


12*7 


* 


i.l* 


7.7 


10.9 


J0*4 


1-7 



3*1. 1 
3.S 
14 1 

t|8,3 
60.0 

60 . 6 
64.0 



3.4' 

3.3 
2,8 



aPP 



0.8 



The binoct&l curve And pUii point of the 
at 25 and of KP 4 PyrUilne * H t n at 
by Ginnings, Herring and Webb, 19^5 an*i itaftiiig?i 
but the authors do not giv* th#?ir exprinnial 
of a series of arbitrary constant ft calculated 
empirical 



KF * fCH 3 ) f Ot)H t HO 

tlet^rwinH respectively 
Aaci Hinottara, 1933, 

but only the values 
the by weans of 



IK TI SYSTKW FOTAIISIUH FMtotroi, 



Results at 30 



(*ns. pr 100 jpw. 


WC. Ml. 


^__^^__ 


"TF** 


1*98 


I..M 


1.20 
0.80 
0.52 


3*53 
6.32 
9*64 


0.40 
0.01 


13*9 
16*8 


"-" 


30.2 


_ 


28.1 





37.5 



iteitif 



1* S3 

n.afi 

, o | 



MC = A aeries of nixed crystal H UoUd 
tion from 0,8 to 1,4 *ols. KF per t ol. 



. 0i 

C- '"\ 



ui8 MC 

11.10 " 

ill^ ^ 

aa!i 

ti 

i?;? 

il . 3 " 

varying in cowj>oi- 



809 



KALIUM K 



POTASSIUM Hafnium FLUORIDE K 2 HfF fi 

100 gms. sat. solution of Potassium Hafnium Fluoride in Water contain 
3.0 gms. K E HfF 6 at 20. (v. Hevesy, 1923.) 



POTASSIUM Niobium FLUORIDE K ? NbF ? 



SOLUBILITY IN WATER AND IN AQUEOUS HF AND AQUEOUS KF SOLUTIONS. 

(Ruff and Schiller, 1911.) 

The determinations were made in platinum vessels. The mixtures were 
shaken for 3 hour j>eriods at constant temperature and the saturated solutions 
filtered through platinum funnels. 

Cms. per 100 Gms. Sat. Solution. 



Solvent. 



Water 

a. 



Aq. 10.95% HF 



Water 
Aq.4-8i%KF 



I> . 


NbF,. 


KF. 


HF. 


16 


S-I9 


2.98 


0-35 


16 


7.07 


5-33 


4-35 


16 


4-33 


2.32 


10.43 


16 


1.16 


5-54 


0.^3 


16 


2.67 


6,04 


S-39 


35 


30.39 


14.68 


0-35 


80 


11.66 


10. 08 


I-S3 



Solid Phase. 



K,NbOP.HtO 



POTASSIUM Phospho FLUORIDE KPF e 

One liter sat. solution of Potassium Phospho Fluoride in Water contain 
0.432 gm. mols. KPF. at 22.5. (Lange and Muller, 1930.) 



POTASSIUM GERMANIUM FLUORIDE 

SOLUBILITY IN WATER. 

(Winkler, 1887; Krust and NUson, 1887.) 



loo gms. H 2 dissolve 173.98 gms^KaGeFg at 18, and 34.07 gms. at 100 (W.). 
100 gms. HjO dissolve 184.61 gms. KaGeFe at 18, and 38.76 gms. at 100 
(K. and N.). 



K KALIUM 



8*0 



POTASSIUM SUico FLUORIDE K f SiF 6 

SOLUBILITY or POTASHIIW SILICO PLUORIDX IK WATER AND 
IK ARROWS AKft ALCOMOLIC SOLUTIONS, 
r an* HarUMorr* ttmj 



The determinations were made at roo tcwperAiure, about 17, The 
mixtures were frequently shaken during several hours and then .ill owed 
to stand over night. The dissolved K f SiF^ WAM determined by titmion 
with o.i N*ftH using phenolphthaline '*a indicator, bringing the solu- 
tion' nearly to the boiling point at th<* end of the tit ration. 



Water 

Aq. so W 

Ag. Sat, 

Aq. Sat. KOI Solution o.oonB 



CJLOH 

Solution 0,0048 



g. KC1 per 



sol. 



A ' ^*> s o.ooaa 

Th ^ *%liove ^ o.^cc 

c> i s* R^i 11,0020 

SOLUBILITY or POTASSIUM Siuro Futoirpi IN VATIR. 



The mixtures were Agitated mechanic Ally for one hour uui Allowed to 
stand 2ff hours At conatant tewperaxure. The solutions w^ri* 
volumetrically. 



tea. K^ F a ptr 
lOOcct tu. oi 



pr 
Wee ami. aok, 




16 
2$ 
35 



0*077 
0.132 
0i?7 

Q.3ft6 



7ft 

8B 



SOLUBILITY or PotASftttm Sluice Futowiot JM 
OF BTHYL ALCOHOL AT m. 



wt. Pareant 
in Soiv 

0.0 
8.7 
15.9 



lit, K^ 
nur A 

0*9 



we. 



J7.| 



iiwr 
0.09 



8n KALIUM K 

POTASSIUM Tantalum. Fluoride K ? TaF ? 

SOLUBILITY op POTASSIUM TAKTALHM FLUORIDE IK 
AQUROUS SOLUTIONS OF .HYDROFLUORIC ACID. 

(Babaeva and Klatchko-Quurvltch, 1935.) 
Results at o Results at 20 Results at Bo 



nms. Der 100 Ctoa. ptr 100 
*ms. aat, sol. Solld tfM. safe aol. 


Sol la 


(Jus. per 100 
gjns. aa^. sol* 


Solid 




"v Phase 


' H 2 


! F 2 


\ 


? Taf 7 


Fftate 


o. 105 


0. 


1 14 KjjTaF 


\ X o. 


214 


0.226 


K 2 TaF 7 * 


X 2. 


170 


3 


.367 


^_TtiF_, 

f 7 


0.6lO 


0. 


2^6 K-TaJ 


' 7 o. 


288 


0.319 


K 2 TaF 7 


5- 


023 


3 


843 




1.757 


0. 


287 


1. 


520 


0.620 


II 


7.550 


4 


305 


11 


3.750 


0. 


364 " 


4. 


234 


0.783 


II 


10. 


230 


4 


863 


" 


6.545 


0. 


'154 " 


9- 


859 


1.015 


II 


16. 


6<>0 


6 


331 


it 


11. 207 


o. 


579 


16. 


520 


i.iino 


II 


24* 


233 


8 


.820 


ii 


17.273 


0. 


815 


19. 


047 


1.609 


11 


32. 


6lO 


11 


,4J4 


H 


2*4.099 


I. 


326 


25. 


420 


2.368 


II 












38.366 


L\.. 


500 


32. 


025 


3.825 


II 


















38. 


157 


6.345 


II 












POTASSIUM Thorium 


FLUORIDE K, 


JhF.-H, 


,o. 













100 gros. sat. solution of Potassium Thorium Fluoride in Water contain 
0.000064 gro. K 2 ThF 6 at 25. (Spicin, 1917.) 

POTASSIUM Titanium FLUORIDE K.TiF-.H.O. 

It v 9 

SOLUBILITY op POTASSIOM TITANIUM FLUORIDE IN WATER. 

(Marlgnac, 1006.) 



Gms. K g TiF e per 100 gms. H 0.55 0.67 0.77 0.91 1*04 1.28 



SOLUBILITY OF POTASSIUM TITANIUM FLUORIDE IK 
WATER AND IN 98 PERCENT ETHYL ALCOHOL. 

(Olnobarg, 103P.) 

Results for Water Results for 98% C^H^OH 



Solid iia, ^t* 1 ** 

per loocc aat. aol. Phase L pr lOOcc at. aoX, l*hMt 

20-22 1.3 K ? TiF fl .H J? 20-22 0.005 K^TiP^j.H^O 

" 1*2 KjJiF e - M 0.0045 w 

POTASSIUM ZirconoFJLUORIDE K 2 ZrF 6 (See also Zirconium salts,) 
SOLUBILITY OF POTASSIUM ZIRCONO FLUORIDE IN WATER. (MlMscmiwt, 19JM.) 

No information is given as to how the determinations wre made and no expla- 
nation of the column heading No of parts of water . Presumably this it the 
grams of water required to dissolve one gram of the salt. 

No of parts No of purlu No of \\nrln 

f- water. t". water. t". wmr. 

10 81.75 4o 42. i5 Bo i4.5o 

20 .... 64 . 5o 5o . . . . 34 . oo go , . . . <j . <K> 

3o.. .. 52.oo 6<>... . 20.25 loo.... 4.yo 
70.... 19.75 



C KALIUM 812 

100 gms. sat. solution of Potassium Zirconium Fluoride ii 
2.6 gro. KgZrF at 20. (v. Hevesy, 1933.) 



Fusion-point data are given for the following mixtures: 

KP + KOH (Scarpa, i 9 i S ** KF * K PO (Amadori, 
* KHV (Amadori, 1913 .) * K g SO (Karandeef, 

" * " " 4 



POTASSIUM IODIDI KL 

SoLuraumr IN WATSR. 

(Mulder, de Coppet, * Etard, ^^^ ^ TWdt a d Shewlooa, ,884; 



. KI per 100 GIIM. ^ Qmi . KI per too Oma. 

Soluticwi. * - C5E 



-io 115 -i 53-5 80 192 65.8 

- 5 119.8 54.5 90 aoD 66.7 

- i 122. a 55.0 100 208 67 5 
o 127.5 56,0 no 215 683 

10 r 3^ 57-6 o 223 690 
20 144 S9-o 

25 148 59.7 Ice <^w 

30 152 60.3 - 5 25.7 22 5 

40 160 61.5 7 42.6 29.9 

50 168 62.7 -9.5 51,5 34 . 

60 176 63,7 -11.5 64.7 39-3 

70 184 64.8 -14 75.8 42.7 

with u* 

by van Dam and Donk (19x1), and by Greeaidi and Smith (1001) g 

or RU-AMION Iow0 x 



The very closely agreeing resuUs of Scott and FnuUr, m r Scott 
andFrazier, 1927 ; Scott and 0urh 1930 ; Hill, WUlson dBU|,S o 
curv! g ' 1936; Wre Pl tted Wd the ^ U ^S vat, taken frS the 



, 

iOO 



20 1 - 

- l - 211 

1(0 " 



OF 



o &* KT pep 

100 M. H^O 

1() 206 . u 



IH WATM AT 

r run STHIUBTIC METHOD. 
osu tanu. ojtotoo, iknur.n ua mnatriieti. MS 7.) 



in 






30 o ' 

' 33 



190 a8a .6 aw 3,8. a 



813 



KALIUM K 



-20 

-22.5 
-23.2 



SOLUBILITY OF POTASSIUM IODIDE IN WATER, DETERMINED 
BY THE FREEZING-POINT METHOD. 

(Kremann and Kershbaum. 1007.) 



22.5 

20 

-IS 

10 

~ 5 
Eutec. ci.o " 4-Ki o 



Gms. KI per 
loo Gms. 
Sat. Sol. 


Solid 
Phase. 


38 


Ice 


41.2 


" 


44.6 


" 


48 


" 


51.2 


" 


51-9 


" +KI 



Gms. KT per 
100 Gins. 
Sat. Sol. 


Solid 
Phase, 


52.1 
52.6 


KI 


53-5 


" 


54-5 


*' 


55-4 
56.4 






SOLUBILITY OF POTASSIUM IODIDE -f IODINE IN WATER AT 25. 

(Foote and Chalker, 1908.) 



Gms. per TOO Gms. Sat. Sol. 


Present in 
Solid Phase. 


' KI. 


I. 


1 KI. 


29-45 


64-34 


34.89 


Kland 


28.91 


63.88 


34-97 


h KI 3 


26.84 
27.18 


66.54 
67.14 


39-70 
39 - 96 


KI 3 and 
KI 7 


27.14 


66.60 


39.46 





Gms. per TOO Gms. Sat. Sol. 



KI. 
25.88 

25-57 
27.86 
27.27 
26.95 

25- 7* 



I. 

68.79 
69.01 
66.56 
66.91 
67.17 
67.91 



The experiments of Hamberger (1906) are discussed. 
For other data upon polyiodides see Iodine 



I KL 



43.44 



Prevnt In 
Solid Phate. 

KI T and 
Iodine 



KI 7 



SOLUBILITY OF MIXTURES OF POTASSIUM 
WATER AT o, 30 

(Van Dam and Donk, 



Results at o. 

Gms. per too Gms. Sat. Sol. 



Agl. 


KI. 


O 


56.1 


9 


53 


18 


51-2 


3 I -3 


46.6 


37-9 


44 


37-6 


42.7 


38 


41.3 


28.! 


36.4 


26.6 


34-6 


6-5 


26.1 


i- 5 


20. <> 


0.2 


9.8 


27.5 


48.7 


21 


50-3 



Results at 30. 
Gms. per 100 Gms. Sat. Sol. 



IODIDE AND SILVER IODIDE IN 
AND 50. 
., 1911.) 

Results at 50. 
Cm*, per j_oo_Gm>. Sat. Sol, c^^jj ph^ i Q 

Each Cue. 

KI 



" H-Afl.lU 
Agl.KI 



' Agl. 


KI. 


AgL 


KI. " 


O 


60.35 


O 


62.6 


16 


55-5 


10.7 


59.1 


35-8 


46.9 


22.8 


5S-5 


42.8 


43-9 


45 


43-25 


44-1 


43-2 


53-4 


37-6 


47-7 


40.9 


53-5 


37- x 


49-7 


38.6 


53-5 


36.6 


42.8 


38.8 


53-5 


36.5 


29.4 


37-6 


39 


38.1 


10 


31.4 


28 


36.7 






16 


33.8 


O.I 


10.2 


2.5 


24. S 



Aft 



AgtaKI 



KALIUM 



SOLUBILITY OF POTASSIUM TODIDK XH AQUEOUS SOLUTIONS 
POTASSIUM IODATE AT 35 ANP VICE VERSA. 
(pled. 10*7.) 





a. of 


OBBS. per 100 


0p. M 


it. Ml 


Solid 


a, or 


OM. p 


>r 100 


{541 8, da 


t. o 


sal. sol. 


' KI0 3 




K! 


Ptiut 


MC. mi. 


r KiOji KI 


1 


.718 


0,0 


$9 


.76 


KI 


1.451 


2 


54 


41 


. 10 


1 


731 


1. 10 


$9 


.1*1 


*i 


1 .^27 


3 


.37 


22 


-38 






2.2$ 


SB 


.62 


*t 





4 


.33 


12 


.04 


1 


751 


2.3$ 


58 


.51 


w * KIO 


8 l "^51 


7 


.15 


2 


40 


1 


.722 


2.3$ 


$7 


.02 


KIO S 


' 1.071 


8 


449 


O 


.0 



SOLUBILITY OF POTASSHW looioi IN AQUEOUS SOLUTIONS or 
POTASSIUM HYDROXIDE AT 20. 



KIO. 



Ota. Hols, ptr liter mit. .HOI. 

.- ,..,-,-,:,- ,-,- >V- - .. 

^ 



di. noli, ptr 



.1 ur MC. 

... ...... _ ..... .. 





9.41 1.72 


13.93 


0.824 


4 


10.95 123 


14.02 


0.672 




11.10 1,176 


1 S . 1 


0*558 




12.19 0,933 








SOLUBILITY or POTASSIUM IODIOR I* 


AQUROUS Sot 


UTIOMS OF 


POTASSIUM SULFATX AT 25 AMD VICE VRRSA. 




d.of <*. Pr 100 . Ml. MX. UDlla d-u 


f **. ttr i! 


PC *. wu noi. soiu 


aa 


t. sol. * iOJK). Kf "^ Wi*i **(.. 


oi. r ""KJJ^ 


"^"' '"Kf* PIlMt 


1 


.718 o.o 59.76 KT i ,37 


^ 1.70 


*S.8i K S8 


1 


.722 0.08 59. 60 "^K^SO^i.ig 


^5 1-57 


lB-57 " 


1 


.701 o.io 58.70 K ft SO 1,12 


17 fu^7 


9,13 H 


1 


399 0.69 39*57 n 1 Cil! 


ll 10.76 


o.o M 




SOLUftltlTY OF POTASSIIIH I0DIBE IN 


Aot'ftous SOLUTIONS OF 




SODIUM IODIPI ANO Vici 


VlISA. 






fNtii, wtiiofl Ma imep. 


19W.) 




t o 


<* Py^jggjy* sat ol. fciia a 


M. p*f 100 ^i* 


tt* -wi. Solia 




/ Kr N&I n PIM l r 


K| 


NAI ^ PftM 


8 


$7.33 o.o KI 35 


,7.59 


S915 KI * NaT.aH^l 




37.54 19.97 " " 


7.06 


59.71 NaI.2H F 




19.20 10.55 M M 


6.80 


59. 97 n 


n 


8*36 $5.58 H 


5-44 


60*74 ** 




7-44 57.13 M + NaJ.aH^O w 


4.78 


6l,35 


" 


5.82 58.23 Nal.aH^O ' n 


a. 17 


63.15 n 


" 


o.o 62.49 M w 


0.0 




2$ 


59.78 o.o KI uo 


6l. 71 


o.o KI 




50.32 9*29 " w 


48 . 04 


13.47 " 


M 


42.08 17.60 H M 


15-55 


26 . ao " 




29.79 30. SS " M 




43.04 " 


J] 


21.43 40.lt 


*.* 68 


57.85 


II 


15.90 46.91 " " 
lo.6r> 54*49 H M 


7.23 


62.14 ^NaLaHjp 

63.93 NaI. 2 H.O 

* r * 



0.0 



8lS KALIUM K 

SOLUBILITY OF POTASSIUM IODID* IN AQUEOUS SOLUTIONS OF 
LF.AD TODIDI AND VICK VERSA. 



Results at 13. 


Results 


at 2.V. 


Results 


at 50, 


)emassieux,1923.) 


( Burrugo 


, 1926. ) 


(Demassieux, 1923. 


(5nis. per 100 gins. 


Gins. p i r 


100 gins. 


(inis. per 


100 gins. 


sat. sol. 


sat. 


sol. 

III|P ,II . 


sat. 


sol. 


KI. IlI a . 


KI. 




KI. 


IM>I.S. 


o.o o.o5 


o.o83 


0.0234 


2.84 


o . 002 


2.21 O..OOI 


o. 1 66 


o , 0092 


9.33 


O.O2 


4.18 o.oo i 


0.332 


o . oo4o 


14.48 


O . O'Jt 


9 . 09 O . OO2 


0.66/j 


O . OO2O 


17.36 


O . I >. 


- 


o . 8 Jo 


0.0019 


18.77 


o. 1 4 


_. 


1.661 


o . oo i 6 


19.50 


o. i5 


__ 


3.320 


O . O02O 


2 1 . 00 


o . 27 


__ 


8.307 


0.0073 


29.43 


1.74 


_ 


i3.6i 


o.o3i6 


29.51 


I . o2 


_ 


14.90 


0.0578 


3o.47 


2.4 > 


_ - 


19.45 


0.253 


3o.57 


2.5'Ji 


6.0-2 o.o5 


21,32 


0.428 


3i.77 


3.H 


7 . 26 o . 02 


26.82 


0.553 


32.12 


3.io 


1.3-2 0.19 


36.73 


1 . 22 1 


36.18 


3-99 


4.45 0.68 


43.8o 


2.349 


38.44 


4.23 


7.25 0.77 


49-43 


3.712 


42.28 


5.64 


5.17 1.47 


5i.6t 


4.654 


51.93 


9 ^9 


2 . 1 4 2.91 


54.6o 


5.876 


53.96 


11.74 


6.55 4-54 


56. 5 9 


7.421 


56. 4i 


x4-*4 


7 . 66 o.o 


57.82 


5.a35 


58,49 


9.72 




59.i3 


5.49 


60.28 


5.55 




59.72 


o.oo 


61.98 


1.5-1 








62 . 02 


1.48 








62.39 


o.o 



Solid Phase, 



PbIi.KI.7HsO 



..- Kf 
KI 



In the case of the determinations by Burrago, constant agitation in a thermostat 
ras employed. At low concentration of Pbl t the load was dotermmod colori- 
letrically. For the determinations by Demassieux tho solutions ware simply shaken 
y hand several times a day and the temperature held constant to within A 

See also PbI, Lead Iodide, for additional data on this ay at em. 



SOLUBILITY OF POTASSIUM Io0inn IN AQUEOUS SOLUTIONS 
OF MKTHYL ALCOHOL AT 25. 

(AKerlor ana Tui-cK, I'r^s.) 

il.% CH^OH (In. Mola. KI per Wt.$ CH^OH On. Hula. KI pttr Wt.tCH^K ika* Hull* K! pr 
n Solvent 1000 9. Solvent in Solvent 1000 tgma. .Solvent In Solvent |OOC W 

0.0 8.962 60. 21 3331 b9.79 1, 

20.0 6.776 72.39 2.^73 9^.76 l. 

40.82 4.8us 80.03 1.970 too.oo 0, 



KALIUM 816 

SOLUBILITY OP POTASSIUM IODIDE in AQUEOUS SOLUTIONS OF 
LEAD IOMDB AND VICE VERSA. 



(Van Klooater ana 8*1 on, 1934.) 



Results at o 

ana. per 100 gps. sac. M l. 

___ 



Solid 



' KT 


Pbr a 


m 


56.07 


0.0 


KI 


55.65 


1.23 


w 


55.28 


2.00 


tl 


55.10 


3.10 


M * KPbl , ; 


53.10 


2.41 


KPbI 3 .aHJJo 


^0.56 


0. 724 


H 


35*20 


. 445 


M 


29.72 


0.263 


tl 


25.56 


0.146 


M 


19.60 


0.074 


H 


15.26 


0* 044 


M 


11.42 


0.037 


H * Pbl 


10,35 


0.030 


Pbl, * 


7.26 


0.012 




4-55 


0.002 


n 


2.21 


0.001 





0.166 


0.003 


it 


o.o 


0.043 


H 



Results at 25 

ptrjpo 41. a*t. oi. 
" 



Solid 



58.53 

58.40 

57,75 
56.60 
55.75 



18.18 

30.77 
2K29 
21.09 
31.01 

I9 . s g 

12.52 
9.97 
0.6t5 
O.J59 
0,00 



0>0 

2,267 

3.66-5 

s . aa ' 

7.30 



1.537 
O.BOJ " 
0.423 " 4- 
0.410 
0.408 



0.001 
0,010 
0.075 



. 



EQUILIBRIHM TK THI SYSTBH POTABSIWM Iooxi f AKTIMOHY ZoDroi ANH WATKR. 

to 381 rrii a Dti*uiU, ww.j 



The authors give a diagram but no numerical r*aiiUa. Thi* following 
approximate values for the triple points were fftifnated from the diagram. 



Results at 16 



160 



Results 



at 48 



230 
200 



130 
H5 



3x8 



200 Sbl ? * 



EQUILIBRIUM IN THI STATIN POTASSIUH FOHI&E, CArniKi AND WATER. 

C^*n HUM Duron, t087.) 

Results at 2 Results 35 Result * at 90 



f car ft rst(iShj0 



18.2 

0.0 



0.0 



133.1 
130.1 



3.52 



0.0 



0,0 



156.0 
156.0 



S3.5 

70.3 
41*0 

43-0 
0.0 



0.0 
5*0 

167.0 

199-0 
196.6 



Caffeine 



KI 



KI 



8l7 KALiUM K 

SOLUBILITY OF POTASSIUM IODIDE IN AQUEOUS SOLUTIONS OF ETHYL 
AND OF METHYL ALCOHOL. (Zeitlin, 1926. ) See last table p. i36i. 

Cm. mols. KI 6m. moli. KI 

dissolved per literal dissolved per HUM- as 

Solvent. 10. 2. 19*. 0. Solvent. H".2. !".. 

a ter 5.863 6. no Aq. 25.96 wi.<Y<>CH n OH. 4.169 4.3oH 

[. 25.07 wl. /o C S H 8 OH. 3.970 4-o83 45.i3 , 3.089 3.2 r > 

5o.oi .2.419 2.612 74.88 . i.(>32 1.693 

75.o3 . 1.120 1.142 100.00 > . 0.7519 o.735(> 

97.30 . 0.042^ 

> gms. glycerol of d == i.2326(= 86.50/0) dissolve 58.3 gms. KI at 20. 

"' ' (Holm, 1021, Itiaiw, lM. I 

OLUBILITY OF POTASSIUM IODIDE IN AQUEOUS SOLUTIONS OF METHYL ALCOHOL 

AT 25. 
(Here and Anders, 1907.) 



Solvent. 


Sat. Solution. 


Solvent. Sat, Solution. 


' . Wt. Per cent 


, Gms. Ki 


' , Wt. Per cent j GUM, KI 


V' CHjOH. 


y per 100 cc. 


<V CH a OH. *V per loo cc 


0.9971 o 


1.7213 102.9 


0.8820 64 I.I&5 40.33 


0.9791 10.6 


1.634 92.12 


0.8489 78,1 I. 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 A..*U*..I*.. 
Gms. Alcohol. Authority. 


Methyl Alcohol 


11.4 


13.5 (TimoWew, 1894.) 


it d 


12. 2 


14.6 4< 


n tt 


13-5 


16 " 


tt 


25 


18.04 (Turner and Bluett, 19x3.) 


Ethyl 


13.6 


1 . 63 (TimoCeiew, t8<j4.) 


n (t 


25 


2. 16 (Turner ami Bwnett, 9ij.) 


Propyl " 


12.2 


0.731 (Timofdew, 1894.) 


tt tt 


25 


0. 43 (Turner and Bisett 1913.) 


Amyl 


25 


0.098 " 



loo cc. sat. solution of KI in ethyl alcohol contain 1.585 gms. KI at 25. 

(Laurie. 



SOLUBILITY OF POTASSIUM IODIDB IN SEVRRAL ALCOHOLS AT 

CLaraon ana Hunt* 1999,) 







** d.of 


Ofem. K\ ptf 


Alcohol 


Formula 


sac., sol. 


100 P>*. fOlvtf 


Methanol 


CH 3 OH 


0.8982 


i7-on 


Ethanol 


C 2 H 5 OH 


0.7977 


1.88 


-Propanol 


CH 3 CH 2 CH 8 OH 


0.8035 


O.IJ44 


-Butanol(n) 


CH 3 <CH g ) 2 CH 2 OH 


0.8071 


0.201 


Propanol (iso) 


CH 3 CHOHCH 3 


0.7821 


0.177 


-Methyl-i-propanol 
-Pentanol 
-Butanol (sec) 


(CH 3 UCHCH20H 
CH 3 (CH 2 ),CH 2 OH 
CH 3 CHgCKOHCH 


0.7986 
0.8112 

0.8026 


0.0955 
O.o89 
0.0582 



K KALIUM 



818 



SOLUBILITY OF POTASSIUM IODIDE IN DILUTE AQUEOUS SOLUTIONS OF ETHYL 





ALCOHOL AT aj. 

l P*tk)fo 



Wt. Per cent 

GH,OH in 

Solvent. 



(Armstrong, Byre, Hututcy. awl Htddfoon, 1907.) 
Wt. Per cent ,/ 

Solvent. 
4-4X 

1.6063 



Sm, Sol. 



jtf (tat. Kl 

liL , per ioo lras. 

Sat. Sol. Sat. Sol 

o 1.7268 59-^0 

1. 14 L7I54 59-41 12,14 

2.25 1.7042 SB.QS X&-73 1.5420 

ioo gms. aqueous 94% ethyl alcohol dissolve 3.99 gm. Kl at 17. 

ioo gms. aqueous 08% methyl alcohol dissolve 17.1 gin*. Kl at I7 e . 

ioo cc. of ethyl alcohol of du - 0.8292 dissolve 8,83 gnu. Kl at i, r e , rf, 4 of sat. 
solution = 0.8989. (Giwmish and Smith, i 



CJms. Kl 

er 100 Cms. 

Sat. Sol. 



S4-Q3 
52.08 

fcuyn, 1892.) 



SOLUBILITY OP POTASSIUM IODIDE IN ABSOLUTE ALCOHOLS. 

(de Bruya Z. physik. Ch, io 783, 'ea; KuhUiui~-Z amirg. Ch. i IJT, *y,) 

ioo gms. methyl alcohol dissolve 16.5 gms, Kl at 20, ^ . 

100 gms. ethyl alcohol dissolve 1,75 gms. Kl at 20.5*. 

ioo gms. propyl alcohol dissolve 0.46 gin, Kl at 15^-20 (R,). 

SOLUBILITY OF POTASSIUM IODIDE IN: 



Ethyl Alcohol 


Aqueous Ethyl 


Aiccihol at 


r 8. 


of 0.^496 Sp. Or. 

. Jt _ _ _ __ A. - -.. . - 




Gms. Kl par 


Sp. Or. 


Weight 


Om*. Kl 


Sp, Or. V 


i/tillii Cms. Kl 


t. 


zoo 


of 


per cent 


per too C5n. 


ol |> 


wr crot pr 100 Oao 




Gms. Mcok>l 


Akohd, 


AhuhnJ, 


Arlwl. 


Alcuhul. A 


kdbt4. Alcdbd. 


8 


67.4 


0.9904 


S.2 


X30-.S 


0.9390 


45 W.4 


13 


69.2 


0.9851 




II9.4 


0.9088 


59 48.2 


2 5 


75- 1 


0.9726 


23 .O 


1OO. I 


0,8464 


86 11.4 


46 


84-7 


0-9665 


29>O 


89.9 


0.8322 


91 6.2 


ss 


87-S 


0*9528 


38.0 


76.9 






62 


90.2 


(Grar4ta Ama. eWm. j 


^f (4) 5. i|$* '65."! 



SOLUBILITY OF POTASSIUM IODZDI IH 
OF SODIUM Ioii AH& or 



The density of the absolute C f H fi OH was cl 
tions were prepared in an atmosphere of hy^ 

Results for tLH.OH ^ 
Solutions of Nal 



a,or 


Twa. pr 100 rf 


M. ''JH-Ol 


SHL. 30l. 

0.7970 


0.0 


^A 
1.824 


0.8215 


4.248 


1.268 


0.8378 


7.091 


0.9988 


0.8502 


9.065 


0,8878 


0.8921 


15.34 


0.6752 


0.9614. 


27.68 


0.442 


1.0500 


43.8 


0.19 



ETHVL Atconot. SOLUTIONS 

s o.78$J The sat. solu- 



R^jiulii for CH OH 
Solutions o ftc? A 



u, or 

Ml. Ml. 

0.8161 



J. 777 

5-13 

6,01? 



0.9182 17.8* 
0*931/1 18.04 



0863* 



50? 
.511 

S6o 

391 

193 
,116 

0,00 



819 KALIUM 

SOLUBILITY OF POTASSIUM IODIDE IN LIQUID METHYL ALCOHOL AT TEM- 
PERATURES UP TO THE CRITICAL POINT. 

(Tyrer, 1910.) 

(Determined by the Sealed Tube Method.) 





Gms. KI per 




Gms. KI per 




Cms. KI per 


t. 


100 Gms, 


t. 


loo Gms. 


t e . 


J.OG Gms. 




CH 3 OH. 




CH 8 OH. 




CHaOH. 


15 


14. 50 


120 


27. 2 


220 


27-5 


3 


16.20 


140 


29.2 


24O 


24.8 


5 


18.9 


160 


30.6 


245 


22.6 


80 


22.5 


180 


30-7 


247 


21 


IOO 


25 


200 


29. I 


2 5 


13-8 








crit. 


temp. 252.5 


7-6 



SOLUBILITY OF POTASSIUM IODIDE IN VAPOR OF METHYL ALCOHOL ABOVE 
THE CRITICAL POINT. 

(Tyrcr, iQxoa.) 



Solvent, 
Gms. CH 3 OH 


Gms. KI Dissolved per 


ioo Gms. Solvent ul: 


per 
i cc. Vapor. 


,_ 


. 


270' 


280. 3tjo". 


300". 


O.I 


O. 


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 


XI. 


5 


XX. 


3 


n 






0.45 


18 


. i 

















Data for the above system arc also given by Oenlnerszwcr (1910). This 
author gives the crit. temp, as 266 and the corresponding concentration as 8.64 
gms. KI per 100 gms. of tne sat. solution. 

SOLUBILITY OF POTASSIUM IODIDE IN MIXTURES OF ALCOHOLS AT 25. 

(Here and Kuhn, 1908.) 



In Methyl + Ethyl In Methyl + Propyl 
Alcohol. Alcohol. 

Per cent <r o f Gms. K* ^ r ^^ rf mB of Gms> - KI 
CHaOH in c fc\ 1** * ce - QfMrOH in y per too cc. 
Solvent. Sat. Sol. Sat. Sol. Solvent. Sat. Sol. Sat. Sol. 


In Ethyl + I'ropyl 
Alcohol. 

Percent rf of Clm. KI 

C|H T OHn L ,l* L . , |r looc'c. 
Solvent. ** **ol- Sat, Sol. 


o 0.8015 1.55 o 0.9018 13 


.16 


o o,Sot$ 


*$$ 


4.37 0.8041 1.91 ii. II 0.8823 10 


.96 


E.I o , 7983 


1 .46 


10.4 0.8071 2.25 23.8 0.8629 8 


54 


17,85 0.79QI 


1 ,37 


41.02 0.8295 4.94 65.2 0.8187 2 


,62 


56,6 0.7988 


0-75 


80.69 0.8794 10.13 9*-8 -$4$ o 


,60 


QQ A A. Q**.JH 

do ,0 O . oO2 2 


0,51 


84.77 0.8795 10.72 96.6 0.8041 o 


.58 


01.2 0,8037 


0.40 


91.25 0.8908 11.84 loo 0.8041 o 


43 


95,2 0.8020 


0,44 


loo 0.9018 13.16 




loo 0,8041 


0.43 


SOLUBILITY OF POTASSIUM IODIDE IN 


ACttTAMXDE. 




(Menichutkin, xgo8.) 








(Determinations by Synthetic Method.) 








J.Q (Jim. KI JHT 100 Solid 


tf> 


Gms. KI iwt too 


Soh.l 


1 ' Gm. Sat. Sol. Phase. 


, 


(im. Sit, Sol. 




82 m. pt. CHjCONH, 


70 


2H.75 


KI 


7 8 6.5 


85 


2Q. I 


M 


74 12.8 


100 


20-45 


II 


70 17.8 


130 


30.15 


*4 


66 21.5 


145 


30. 5 





58 26.2 


x6o 


30.8 


M 


53 Euicc. 28,4 * +KI 


175 


31.1 


M 



KALIUM 



820 



SOLUBILITY OF POTASSIUM IODIDE IN ACETONE AND IN PYRIDINB, 

(von Lascynski 1894; at 25, Krug and McKlroy, 189;,) 

Gms. KI per 100 Gm. Solvent at: 
-a.j e 10 23* a,i* 56* 119* 

Acetone 3.08 ... 2,38 2.93 1,21 

Pyridine ... 0,26 ... ... ... o,n 



Solvent. 



100 gms. glycerol dissolve 40 gms, KI at 15.5. C^eadowskS, 1907,) 

100 gms. 95% formic acid dissolve 38.2 gm. KI at x8>5 . (Aschan, 1913.) 

100 cc. anhydrous hydrazine dissolve 175 gnu. KI at room temp, 

(Weltb ami Broctonon, 1915.) 

ioo gms. hydroxylamine dissolve 1 10 gms. KI at 17.5*. (de Bruyn, 1892.) 

100 gms. sat. solution in hydrated lanolin (containing 30% emulsified water) 

contain 42.5 gms. KI at 45. (Klooe, 1907.) KI is Insoluble in anhydrous 

lanolin. 



SOLUBILITY OF POTASSIUM IODIDE IN SEVERAL SOLVENTS. 

(Waktai, xo6.) 



Solvent. 


Formula. 


r. 


Sp. Gr, f 
Solution. 


CipfiiH Kl per too 


tc. Suluttun. (Jms, Sclution. 


Water 


HaO 


o 


X, 


66<x> 


94 


05 


56, 


32 


Water 


HgO 


25 


I , 


7254 


102 


70 


59- 


$4 


Methyl Alcohol 


CHtOH 


o 


O, 


8064 


1 1 


6x 


12. 


95 


Methyl Alcohol 


CHaOH 


25 


o. 


0003 


13 


5~i4'3 


14, 


07 


Ethyl Alcohol 


CfH$OH 


o 


o, 


HoH^ 


I 


197 


I , 


479 


Ethyl Alcohol 


CAOH 


25 


o. 


7908 


i . 


Sao 


I , 


022 


Glycol 


(r>tJT fMJ"\ 
\* JtJ.2 V/AA/ 2 


o 


I. 


3954 


45 




| t 


3 


Glycol 


(CHsOH), 


2 5 


I . 


38BH 


47- 


23 


33- 


01 


Acetonitrile 


CHsCN 


o 


0. 






852 


2, 


2 59 


Acetonitrile 


CHsCN 


24 


o, 


793$ 


X. 


57 


2, 


003 


Propionitrile 


CtHiCN 


o 


o, 


8005 


o, 


34-0,41 


O. 


OA20 


Propionitrile 


CaHiCN 


25 


o. 


7821 


o. 




O,O404 


Benzonitxtte 
Nitromethane 
Nitromethane 
Nitrobenzene 


Iff 


o 
25 


I. 

X. 

I, 


0076 
1627 
1367 


0, 

o, 
o. 
o, 


051 

314-0,366 
289-0.349 
0019 


O, 
O, 

o, 


0506 
3X5 
307 


Acetone 


(CH'),CO 


o 


o. 


8227 


X, 


732 


2, 


105 


Acetone 


(CHi)jtCO 


2< 


o. 


7^68 


X , 


038 


X, 


3O2 


Furfurol 


cjayo-coH 


O 






15. 


xo 




nj"* w 


Furfurol 


dHiacOH 


2$ 




2014 


5. 


62 


4. 


94 


Benzaldehyde 
Salicylic Aldehyde 
Salicylic Aldehyde 
Anisic Aldehyde 
Anisic Aldehyde 
Ethyl Acetate 
Methyl Cyanacetate 
Methyl Cyanacetate 
Ethyl Cyanacetate 


CJHsCOH 
CeBU.OH.COH 
CeH4.OH.COH 

CeH4.OCHs.COH 
OH4.0CH 3 .COH 
CHaCOOCA 
CH 2 CNCOOCH| 
CH 2 CNCOOCHs 
CHsCNCOOCaHi 


O 
O 

o 

25 
25 


X. 
X. 
X. 


0446 
1501 

1373 
1223 

00 

1521 
o6aS 


o. 

X, 

o, 

X. 

o. 
o. 
3- 

2. 

o. 


343 
257 
S49 
520 
720 
0013 
256 

459 
989 


o, 

X. 

o. 
1. 
o. 

2, 
2, 
O. 


093 

483 
355 
644 

827 
93<> 



821 KALIUM 

SOLUBILITY OF POTASSIUM IODIDE AT 20 IN SEVERAL SOLVENTS CONTAINING 

DISSOLVED IODINE. 

(Olivari, 1908.) 
Gm. Mols. KI per Liter in Solvent Containing: 

Solvent. sGm. Mols. ^Gm.~Moi<r"^^ 

I s per Liter. l a per Liter. la per Liter. 

Acetic Acid 0.511 i . 460 2 . 080 

Ethyl Acetate o . 490 i . 400 i . 980 

Ethyl Alcohol 0.520 1.220 i. 730 

Nitrobenzene 0.414 0,960 1,380 
Ethylbromide 0.140 -35o 

SOLUBILITY OK POTASSIUM IODIDE IN AQUEOUS SOLUTIONS 
OF ETHYLKNE GLYCOL AT 30 - 

roinnlngs and Rottblna, 1030.) 

a. of nms. per_jpO_fl ; _sat._aol. d-of 





sac. sol. cHgOHCHgOH ^ 

1.7302 0.0 60.31 *5395 32.27 4-5'lB 
1.6655 8.96 $5-90 1.4687 Sl-57 3B.37 
1.6031 19.26 50.98 1.4272 66.ni 33.59 

SOLUBILITY OP POTASSIUM IODIDB IK PURE ACBTONK DETERMINED 
BY SPECIFIC CONDUCTIVITY MEASUREMENTS. 

(I,anrmntt, 1932,) 

Q d.of Ons. KT ptr 

L aec. sol. 

l8 0.799 11.19 

37 o.77 B.02 

EQUILIBRIUM IN THE SYSTEM POTASSIUM IODIDE, TERTIARY 
BUTYL ALCOHOL AND WATER AT 30. 

(Glrmlngs and Bobbins* 1 9 TO.) 

The points of the binodal curve of this system were determined by ob- 
serving the appearance or disappearance of clouding in mixtures of 
weighed amounts of KI in one of the liquids upon addition of weighed 
amounts of the other. Tie lines, *, connecting conjugate points were 
located by determination of KI in liquid layers in contt with each 
other and from these the plait point, PP, was found by plotting* 



Oroa, per 100 ano. sac. ol. !5!!lJE^^ 

' "* i ^ 



3-3 54.7* 17.9 39-6 nS0 

a.o 52.9 19.9 3B.6 46,5 

5.2 n9.B 22.1 37.0 4.9.2 

7-2 47-3 2/1.2 35.6 50..0 

47.1* 26.0 ^4.6 PP 52.0 30.*) 

8.4 46.1 27.6 33*4 57.7 18.-5 

9.6 45.4* 10.6 31.9 60.3 l6.9 

11.3 44.0 35.1 29.5 63.8 1S.5 

13.9 42.3 39-2 27.0 63.0 

15.1 41.1 i|2.0 25.5 

l6.6 40.3 44-3 24.6 

The composition of the plait point PP at as is 38,4 gm*. KT * aa.a 

gms. (CHjl^OOH per 100 gms. sat. solution, (Ginning*, Herring And Wehb, 
1933-) 



K KAUUM 822 



DISTRIBUTION OF POTASSIUM IODIDR AT 17 HI*:TWI-;I-;N WATKK ^NI> AMYX. ALCOHOL 

I \V0*nitfttitftk\ i tta;,| 

HllUmol*. tU fiw mpr*-tf ^ 




ioo cc. sat solution of potatRtum icttlidU* in ethyl u re than contain 5.8 1 gms. KI 
at 60. (HUirkgoW, ion.) 

EQUILIBRIUM IN THE SYSTEM POTASSIUM IODXDB KTII YL KTHRK - - WATER AT 20, 

(DuMtinghftm, 1914.) 

Cms, per ioo Gro<. Uj>iwf Layer._ tSmi |*rr too Cii. !<iwrr layer. j^y 

S3! ~" HA (C|Hi)|Ol -* --^^ ^^ 

S^-2 40 8 . .. KI 

o 3.9 $6.1 O .. 93 7 N^ 

0.4 0.4 90,2 55.6 40 7 3,7 KI 

o.i 2.2 97,7 15 7- * 3.t) None 

DISTRIBUTION OP POTASSIUM famine HETWKKN WATER AND; 
Nitrobenzene at xS. {l>&wn, I^OH.) Phtmol at Ktx>m Temp. 

Mob. Kljpyr Utyr. 0^, (m*i. K! irr toorc, 



0.00114 6*05 5300 0.05.1 0.735 i^.a 

o. 00x08 6,0$ O.IQ7 J.4J* i|. .3 

2.0) jo 7 14 7 



Soumum or fVtTAAnH looxint JK ? ALUYI, 
HH or SODIUM !o&x&* AT a^ tt . 



The density of the Allyl Alcohol, C 
fl.of OM. ^tr tOO fi* COi ft O J.of 



wt. sol. il^ ,...,^,^,^ n ^^ ^^ ^..^u^.^...^.. ,.., ^,.,,, 

0,85080 0.0 ***33 0.0075^ S.lfiti 0.7*15 

0.8613^ 11$7 Io6o 0,*||5CJi ia*$CI 0.561 

0.87386 2i^S 1*000 0*06451 17*530 0*;ito 

0.88750 5*100 o*B'i7 o.oS^^a *iJ5a 0.200 

0,88890 5*321 o.Hao 1.02^85 arB.uft o.o 

0.900414 7. 1 10 078l 

So LOB rum or POTASH!*!*! looiot i Pttt BKHXYU 
SOUITIOHS or Sonnm fo&ipx AT 35 



The density of the Benzyl Alcohol C. H CLOH. 

r P 

iJ.gf ftan. ptr 100 tfii, CJI-Ch-OU j.wf f^i 



1.04485 o.o 0,^20 i* 10613 i*6n w*^7^ 

1*05650 1.334 o.ios UU03J 7,367 0.363 

1.06203 a,23s 0*301 t*iaSs u.oio 0.197 

I* IOOIJ3 i|700 0.300 



823 KAL1UM K 



SOLUBILITY OF POTASSIUM IODIDK IN AQUEOUS 
SOLUTIONS OF URKTHAN AT 25. 

(Pftlitswich, 1928. 19?9.) 

Ota. Mola. per^lOOO gws. H g O Solid 

KI ^"""^ Phase 



o.o 9.0355 KI 

U1225 8.979 " 

20.79 8.73 " 

46.72 9.66 " * NH-OOOC-H. 

53.09 o.o NH g COO(yi/ 

SOLUBILITY OF POTASSIUM IOPXDB IN LIQUID AMMONIA. 

t n*a. KT per 100 pis. NH 3 Authority 

o 184.2 (Linhard and Stephen, 1933, 1934.) 

25 182.0 (Hunt, 1932.) 

100 gws. Liquid Sulfur Dioxide dissolve 41.3 gms. KI at o. (Jander 
and Ruppolt, 1937. > 

Data for equilibrium in the System KT -f S0 ? are given by Wai den and 
Centnerszwer, 1903. Results for the vapor pressure, temperature rela- 
tions of the system are given by Foote and Fleischer, 1931, 

Fusion point data have been determined for the following mixtures. 

KT K p S0 4 (Ruff and Plato, 1903.) 

" AgT (Sandoninni, 191 2) 

" * NaCl (Ruff & Plato, 1903! Waxberg, 1930. 1 

" * Pblj, (van Klooster and Stearns, 1933.) 

11 + SOj, (Walden and Centners?;wer, 1903. ) 

POTASSIUM IODOMERCURATE (Thoulct Solution). 

A sat. solution at 22.9, prepared by adding KI and Hglg in excess to water, 
contained 8.66% K, 22.49% Hg, 52.58 (57.7) % I and 10.97 (".5)% IM>, 
corresponding to 0.22 mol. alkali, o.n mol. lig and 0.45 mol. I. (l)ulxin, iyos.) 

POTASSIUM IODATE KIO^ 

SOLUBILITY or POTASSIUM IODATJI IN WATRR. 

The results of Kramers, \8s6U); Marburg, 1905; Flttitm&n, 1928; Hill 
and Brown, 1931; ^"^ Ricci, 1931; above ioo Bonrath, Gjedebo, Schlff^rn 
and Wunderlich, 1937; were plotted and the following values taken from 
the average curve. 

t o a -f * 3 ptr d.of (lis. KIO^ ^r fta KIO, r 

8ftU SOl. 100 |JS. a&C. SOl. l Ml. 01. ICO 4U. Alll. Ql. L 100 8. 9. Ml. 

"""" <*'! 30 ~ 9-1 125, *75 

5 1.043 5-1$ 40 ii. a 150 32, a 

10 S-9 50 l.UO 13.3 17S 17,0 

15 1.0584 6.68 60 15.5 200 qi,* 

20 1.06/13 7.48 Bo 19.9 250 t9 f *8 

25 1.0708 8.40 100 3<|.tj 300 $B,0 



KALI DM 
POTASSIUM Hydrogen 



Compound 

Potassium Hydrogen lodate KH(T0 3 t ? 
H Di hydrogen M KH^iIO^l 



SOLUBILITY or F.ACN in VATIR. 

On. fnj 
fomuU t 



ptr 



Authority 



17 



5.4 



1891, 



EQUILIBRIUM IN THE SYSTEM POTASSHW IODATK, loan: Acm, WATKK AT 30 

(Mcvrlmri, i*tejj 



Cms, per 100 Cms. 
Sat, Sol. 


HID,. 

0.65 

0.67 


9-5* 

9-49 
8.90 
6.6 


1. 14 
1.69 


4-57 


2. 02 


3.10 


3-34 


2. ID 


5 


1,32 


7.09 
8.04 


X 
0.85 



Solid! 



r too Ctffti. 



HttV 


___> 


J-17 


5-50 


4.80 


a,c>o 


!i 


0.64 


U 04 


0.44 


17 ^ 


o. jo 


3 1 jo 


O. ^1 


SJ f>4 


o 6K 


6j 51 


0.71 


76 40 


o 80 


76,7 






i HIO, (unstable) 



100 cc. anhydrous ilytlraimc tikmilvt I gin. KIOj at rm.*m fc*mp. 

|Wf!*Ii ami I 



Hit), 



a. of 
aai. 

ol. 



U043 
1. 060 

1.090 
1.110 
1.120 
1*100 



S0UJIILITY 0r POTA8SIWM !00ATS IH AOtlftOtlft S'liliTIOMS OF 
POTASHXttH NlTftAfl Altt tfl VnmiA. 

IMIII wi4 iffttfi* ti^i,! 

HB8. Dr 100 i ,, :: * s . fr f im 

gain. AH. MJL 



Results at 5 

0,00 1*35 ^10^ 

10*53 2-^3 
*3S! 



2l? 
14*43 00 



as" 



o.o . 
$.48 5*<1 



RIO 



1.110 



4*57 



.167 

.11 
.17 



47. J* J.li; 



KIO * KNO 



KMO. 



825 KALIUM 

POTASSIUM IODATE KIO :) . 

SOLUBILITY OF POTASSIUM IODATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM HYDROXIDE AT 20. (Bronsted, 

Gins. mole, per liter. Gins. mols. per lliw. Cms. mols. per liler. 

KOH. KI0 3 . KOH. K10 3 . ROM. KI0 3 . 

4.71 0.0890 7-95 0.0179 ii. 10 0.0128 
5.o6 0.0862 9.41 0.0144 is. 19 0.0181 
6.35 o.o2$6 10.95 o.oi3o 12.9-.* o.oi35 



<Jms. mols, por lllor. 
KOH. KU) U . 

i4-'^ <>.oi54 
14. 8/5 0.0194 



SOLUBILITY OF POTASSIUM IODATB IN AQUEOUS SOLUTIONS OF 
POTASSIUM SULFATB AND VICE VERSA, 

(Hill sua Rlccl. 1031.) 



d.or 
sat. 
sol. 



ORB. per 100 
3*8. aat. sol. 



Results at 5 



Solid 
Phase 



d.of 
a at. 

301. 



Gtas. per tOO 
pis. sat. sol. 



Solid 
Ph&se 



Results at 25 (con.) 



1.043 


0.0 


5.16 KI0 3 


1.103 10.10 3.44 


i.o6o 


4*07 


3. 14 w 


1.083 10.76 o.o 


1.081 


7.08 


2.57 * K,S0 4 




1.077 


7.25 


1.80 4 


Results at 50 


1.062 


7.64 


0.0 * 










o.o 13.21 


Results at 25 


7.90 8.68 








11.43 7.39 


1.071 


0.0 


8.45 KIO, 


12.0 7.06 


1.085 


4*75 


5.66 


13.0 3.78 


1.103 


7.74 


a. 72 


14. -l8 0.0 


1.117 


9*65 


4-30 " + K SO 





d.of 
sat. 
sol. 



1.043 
1.051 
1.060 
1.046 
1.028 



1.071 
1.098 
1.126 



KICL 



10 



SOLUBILITY OF POTASSIUM IODATE IK AMUKOUS SOLUTIONS 
SODIUM TODATE AND VICE VRRSA. 

(Hill and Rlccl 19S1.) 



QMS. 
8a. 


pr 100 
sac. sol. 


Solid 
Phas* 


^aIO_ 

3 


KIOJ, 


Results 


at 5 




0.00 

1.41 


5.16 
4.71 


KI B 3 


2.17 
2.48 
3.28 


4-72 
3.19 
0.0 


"+NaIO,. 5 l 
NalO.j.sBj.O 


Results 


at 25 




o.o 
4.26 
7.13 


8.45 
7.09 
6.73 


+Lo H 



sac. 

sol. 



Hw. p*r 100 
soi. 



Results at 35 (con. \ 



1. 101 

1.074 



7.79 
8.57 



3-79 

o.o 



Results at 50 



o.o 

3.93 

7.70 

10.92 

11.41 



13.31 

11.92 

1 1. 14 

I0,6l 

7.93 

424 

0.0 



POTASSIUM PerlODATl KIO 4 . 

100 gms. H 2 dissolve 0.66 gm. KIO* at 13, d y of sat. solution - 1.0051 

(Barker, 



K KALIUM 



826 
SOLUBILITY or POTASSIUM PIRIODATE IN WATER. 

(HUl, 19U 



15.0 
25.0 



100 OM. . sol. 

0,169 

' 21 
0.334 



50 
*S 

97 



nan. KIO ptr 

loo ^ H0 



3-59 
6,83 



EQUILIBRIUM IK THE SYSTEM POTASSIUM PBRXODATR, 
POTASSIUM HYDROXIDK AHD WATER AT 25. 

(Kill, 19U 



d,or 
sat. sol. 

1.000 
1 . 04/ 

1.087 
1.1 16 
1.16$ 

1.221 



fltaa. per tOO 
-_ 

0.0 
1 .01 

1.99 

2-SS 
4-55 
6.03 



:wiU Ml, 



a. of ON*, ptr too 
i*U ul. r "-"-- 



o .51 

4. 12 

8-03 
10.32 
13.15 

l6, 12 



KIO. 



POTASSIUM Di-meso- Per IOOATK 



1.336 

1.J77 
1 1 . 6 



.* 



V-7 

11.9 



~t'oTj 

30.8 
2.l 
28,9 

39-0 



_oi. soiia 
"""^ Phase 



SOLURZLtTY Of P&TASSIPM Dl-HISO-PiRZOOATS If* WATI8. 



0.3 1.032 
IS. 1.073 

25.0 1,118 

37.5 1.216 



p@r tOO ips. 80114 

JMIU Ml. PAM 

3,5 ^1^0.9^0 
7.7 " 

12.3 w 

22.0 " 



5 o 
65 



ptr 100 

4t. Mil. 



it Stolid 



1095 15.0 K 1 9 H 

30,1 " 

61,7 w * K I 

6l.7 & 4 * r O 4 f g 



POTASSIUM PerlOOATE 



OF POTASSIUM HITA PRRIOOATS tn 
Aqoious SOLUTIONS or Pit 1001 c Acxn AT j w . 



Ht. Wl. 


^_^ 


* 4 


1*000 


0.0 


0.5* 


1.033 


2*8;3 ? 


0.26* 



K!f> 



82? 
POTASSIUM PERMANGANATE KMnO<. 

SOLUBILITY IN WATER. (Baxter, Boylston, and Hubbard, 1906; Patterson, 1906.) 



KAUUM 



Gms. KMnO 4 per 100: 



Cms. KMnO< per 100 : 





* . 


Gms. Solution. 


Gms. 


H 2 O. 


cc. Solution (P). 


b . , / ^~ ~ 

Gms. Solution. 


Gms. 


H 2 U. 


o 




2-75 


2. 


83 


2.84 


34-3 


9 


64 


IO. 


67 


9 


.8 


4-13 


4- 


31 




40 


ii, 


.16 


12. 


56 


IS 










5,22 


45 


12, 


73 


14, 


53 


19, 


,8 


5.96 


6. 


34 




50 


14, 


45 


16. 


SQ 


24- 


8 


7.06 


7- 


59 




55 


16, 


.20 


19. 


33 


29. 


8 


8.28 


9- 


03 


8^9 


65 


20. 


.02 


25. 


03 



Sp. Gr. of saturated solution at 15 1.035. 

Determination by Worden (1907), made with extreme care, gave results in 
very close agreement with the above. 

SOLUBILITY OF POTASSIUM PERMANGANATE IN WATER. 
( Voerman, 1905, 1906. ) 



0.18 


Gins. KMnOt 
p<*r loo gins. 

- ~~~~+*^-^*~~-~~-^ Solid 
snt. *ol. wnlor. IMiase 

o 58 0,58 Ice 


Cms. Ii 
per HK> 

t". snt. sol. 

~f-i<> 4 .01 


v^--**-""" %. 
HJiler, 

4 72 1 


Sutid 

!*lt*M>. 


0.27.. . 


O.()<) I .0 1 




5 . 7O 




0.48 . 


I.q8 1.0'> 




7 r >3 





0.58 Kmec. 


?.. i) i 3.oo ~hKMn 


Qj. 4 ii .ot) 











5o i^.3"> 


rO -^ 





SOLUBILITY op POTASSIUM PBRMANGANATK IN WATKK* 



t 


d.of 
sac. sol. 


0. KMn0 4 pr 
1CK) #10. c. sol. 


15 


1.0342 


4-997 


20 
25 

25 


1.0397 
l.0a6l 
1.0461 


7.079 
7.097 



FOtnO 



" (Trimble, 1922.) 



SOLUBILITY OF POTASSIUM PERMANGANATE AT i5 IN AQUKOUH SOMTTIO.NK or : 

(Trimble, 102? ' 



Potassium Sulfate. 



Sodium Sulfute. 



'' f 


Gms.pei inogms. 

NUl. S()l. 


tt n of 


Ctrns, par 

MI. 

^'**~*^N TO X 


moim.. 


sat. sol. 


'^soT^^'^*^" 


KMn0 4 . Phiwo. 


*u. not. 




'KMn0 4 , fe * "|h 


.0454 


o.o 


7.10 KMn0 4 


i .0.554 


O!BH 


7.3'i KMnO; 


.0483 


0.80 


6.59 




4 6u 


7.81 > 


.0537 


J .98 


5 . 9 >. 


1. 11*0 


7,o r > 


7 .""> 


.0780 


5..f7 


4. 5 7. ') 




9.34 


7.67 .. 


.0876 


7-79 


3.87 




12.8") 


7.27 


-0979 


9 . 9.6 


3.53 w^KjSO 


4 


17.0'") 


6.68 


.o86| 


10.7") 


o.oo KjS04 


I.2H63 


19.43 


6.'jT> > 










r . 04 


5.91 .\ 








i . '>x>7 1 


a i. Ho 


o.o NftvSOt 



- m ~,*, j m *, , +lir 1,lf JHi,J,f1f^,J^|jnif 

The author also gives data for thft dennities of aqueous solutions of KMn () 4 , KjS 
and of Na a S0 4 . He also gives a few determinations of the solubility of K Mu < 
in aqueous solutions of mixtures of K, S0 4 an<l Na a S() 4 . 



K KALIUM 828 

SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS OF 

POTASSIUM CARBONATE. 

(Sackur and Taegener, 190.) 



Mob. KMnO 4 per Liter in: 
.-* .,.,, . ,,..,, 





o.i w jKC*Oj. 


i n IK^COg. 


3 n iK,a) a . 


4 n iK,CO. 


6 n JKjCO 


o 


0.1462 


o . 0629 


o . 0446 


O.027 


0.0156 


25 


0-4375 


0.2589 




O.OQ3 




40 


0.7380 


0.5007 


0.3519 







SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM CHLORIDE, 

(Saekur and Tmegener, 191 a.) 
MoU. KMnO per Liter in: 



t*. 


o.i n KG. 


0.5 n KC1. 


i n KCl 


j KC1 


o 


O.I39S 


0.076 


0,0532 


0.0379 


25 


0.4315 


0.306 


0,22O 


0.1:432 


40 


0.738 


0.584 


0,444 


0.288 



SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM HYDROXIDE, 

(Sackur and Taegencr, 191 a.) 
Mob. KMnO< per Uter in; 

MnO 



t". 


H 8 0. 


i n KOH. 


a n 


KOH. 


4 n 


KOH. 


6* 


KOH, 


8 If 


KOH. 10 n KOHL 





0.176 


O.OSO 


O, 


031 


O, 


027 


O. 


023 





,017 


0.0X2 


10 


0.278 


0. 112 


O. 


068 


O. 


048 


O. 


O42 


O 


,028 


0,016 


20 


0.4II 


0.179 


0. 


1X9 


O. 


079 


O. 


074(*S 


) o 


.032 


0.029 


30 


9-573 




") o. 


2I3(ja 


o, 


, I4C)(J2 


o, 


114 


o, 


,06200 


0.040 


40 


0.792 


0.439 


o. 


306 


o, 


211 


o. 


161 


o 


,084 


0.052 


50 


1.154(53*) 


0.638 


o, 


462 


o, 


304 


o. 


219 


o, 


, III 


, , , 


70 


i. 812 


1,172 


o. 


869 


o. 


572 


o. 


39 


o, 


, 188 


0,082 


80 




I.5I3 


X. 


X90 






o. 


$00 


o, 


,231 




90 














o, 


649 


o, 


,297 





SOLUBILITY OF POTASSIUM MANGANATE IN AQUEOUS SOLUTIONS or 
POTASSIUM HYDROXIDE. 

(Sadiur and Taetfencr, itfu>) 

(The KjjMnOi was prepared by boiling KMnO< with very cone. KOH, draining 
by suction and washing with ice cold Rt(.X)> solution. The impurities were of 

BO consequence since the determinations were made in alkaline solutions.) 



Moll. KMnO< per Liter in: 



t*. a KOH. 4 w KOH, 6 m KOH. ft n KOH, 10 KOH. 

o 0.907 0,554 0.155 0,063 0,0145 

10 1.013 ... . .. 0,070 0.0152 

15 o.68xd7*> 0.224 

20 1.140 -733( J s*) 0.261(3,1*) 0,078 0,0160 

3 1.252 0.772 0.303 0,096 0,0215 

40 .-. 0-^S 2 0.362 0,119 0-030S 

45 1.424 0-889 0.388 

5 ... 0.938(51*) . .. 0,142 0,0462 

60 ... 2-003 0,469 0,167 0,062 (6j*) 

7 ... 2.074 0*5^8 0,196 0,070 

80 ... I-I43 0-5^7 0,222 0,083 

too cc. anhy. hydrazine dissolve 2 gms. KMnOi, with evolution of gas and for- 
mation of a brown precipitate, at room temp. (Wit* md Brcckmoa, 19*3.) 



829 



KALIUM K 



POTASSIUM Per MANGANATE 



SOLUBILITY OF POTASSIUM PERMANGANATE IN AQUEOUS SOLUTIONS 
OP SALTS AT 25. 

(Here and ill eben thai* 1929.) 
Results for Aqueous Solutions of: 



Lithium Chloride 
Oku. MoU. per liter 


Sodium Chloride 
Q. Mols. j?er liter 


Ammonium Chloride 
Dm. Mols. per liter 


' L1C1 


l/*-KMn0 4 V 


'Naci 


1/iHOttO/ 


/ _--_- - 


l/.lrXMnO, 


0.0 


2.25 


0.59 


2.32 


0.$9 


1.9q 


0.51 


2.18 


0.96 


2.29 


0.9S 


1-75 


0.87 


2.09 


2.26 


2.13 


2.69 


1.05 


2.56 


1.51 


3-35 


1.86 


3.78 


0.86 


3.8l 


1.16 


4.22 


1.73 


*JS7 


0.78 


4.S6 


0.95 


+ $15 


1-53 


+5.4.5 


0.72 


Magnesium 


Chloride 


Calcium 


Chloride 


Stron ti urn 


Chloride 


(*. Mols. 


jper liter 


dta. Mold, per liter 

, >\ 


(Tm. My la. 


p&r !Hr 


0.96 


2.01 


0.0 


2.35 


0.0 


i/vwno 4 


1.92 


1.78 


1.70 


2.00 


0.64 


2.27 


4.62 


0.96 


4.90 


1.20 


2.45 


1.94 


6.42 


0.64 


6.80 


0.91 


3-92 


1.6f| 


7.64- 


0.48 


8.10 


0.80 


4.52 


1.50 


8.10 


0.40 






+5-90 


1.16 


+9.52 


o. 16 














Potassium 


Chloride 








(1m. MolS. 


j^er llttr 


On. Mola. 


.jjr uitr 






' KC1 


i__^ 


rm -'-- 


" i/^tHftd^ 






0.36 


1.56 


2.32 


0.58 






0.6l 


1.30 


2.89 


0.51 






1.65 


0.74 


4,06 


O.qO 





SOLUBILITY OP POTASSIUM PERMANGANATE rw AQUEOUS SOLUTIONS 

OF ACETONB AT 13. 
(Htra; ana Knock., 190^,) 



CC CH^COCH^ 
per lOOcc solvent 


per tOOcc sat. sol. 


ec rH^CQCH, ( 
ptr tOOee solvent 


Ows*. HMnO, 
ptr lOOcc nat. 


0.0 


4-70 


60 


10, OP 


10.0 


5-13 


70 


10. ^8 


20 


5.6l 


Ho 


g . B<> 


30 


6.59 


go 


7.18 


40 


B, 14 


100 


2. ia 



KALIUM 830 

SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM PERMANGANATE AND 
RUBIDIUM PERMANGANATE AT 7. 

(Muthmarm and Kuntzc, calc. by Fock.) 



Milligram Mola. per Liter. 


(Jms. iM-r 


Liter. 


Mol. per cent 
KMnOj in 


JCMnb,. RbMnO,? 


' KMnO 4 . 


RhMnoT 


Crystals of Solid 
Phase. 


27,04 22.6() 


4-28 


4.64 


3 - SO 


75 22.22 


11,84 


4-54 


13-75 


120.26 31. 2C) 


IQ.03 


6.40 


34-20 


188.30 3^-OB 


2(),Ho 


7.Q7 


7^45 


198.36 4*- 2 <> 


31.30 


8,44 


92.50 


205.76 42.50 


32.56 


8,6c) 


90.47 


225.12 26 


35 -61 


5-32 


OQ.32 


264.27 o 


41,81 


o 


1OO 



POTASSIUM MOLYBDATK K|MoO 4 

SOLUBILITY OF POTASSIUM MOLYBDATK IN AQUEOUS SOLUTIONS OF POTASSIUM 

SULFATB AT 25 AND VlCK VERSA, 



(Amadbn, l 

Cm*. per oo Oms. _ HA_ 
_ i,_ 



o 184.6 1.50 t.X).49 

0.46 180.7 2 -M 45 -8<) 

0.72 177 3-95 s 7-48 

0,98 127,2 8.55 4-73 

1.27 107.5 !2,lo o 

Freezing-point data for KiMctO4+ K S SO 4 , KtMuOi + KfWOi and K t MoaO 

arc given by Aniatlori (1913)* 



Results for K,Mo0 4 * MoO, .mil K f Mot) 4 * Li p Mo0 4 tml K^WT> 4 * Vf0 3 are 
given by Hoertnann, 19319. 

POTASSIUM PHOSFHOMOLYBBATE K.P0 4 . 1 1 MoQ. I JH*0. 

TOO g:ms. HjO dissolve 0.0007 gm. at 30. 

100 gms. aqueous 10% HNOi dissolve 0*204 gm. at 30*, (Doak, M. 0., 1905.) 

POTASSIUM PHOSPHOMOLYBBATE 

SOLUBILITY OF POTASSIUM Pa<>HmoMot.Yiii>ATr IN At|r*'',m:h SfH.r-no.NS 

POTASSIUM NITIIATT, i H4tiwh*tln, IWIH.) 



In order to avoid errors tlw tc iiu|urltir8 in I he* phoHphomoIyhciniCi small 
quantities of the washed jmuipittttr \vtrs <lig*^tiH.i for a tim lung tMiaugh lo insure 
saturation, and the ditsoivcci part dotormtuttd either by rvnporatton and weighing 
or by titration. Tho toiupAriiturt* is not 




ll. WltlltifH). 

o . t ? 
0.18 



POTASSIUM PHOSPHOTUNGSTATE 

looo cc. sat solution of potaftium phoHphatttttgHtutc in \vwlcr coutuiu o.iSI gm. 
of the compound at ao. I Mowi- *ml WIHCIM*!, HI-B.) 



831 KALIUM 8 

POTASSIUM AMIDE KNHg. 

100 gms. liquid ammonia dissolve 3.6 gms. KNH p at 25. (Hunt an. 
Honcyk, 1933. ' 

Data for the freezing-points of mixtures of potassium amide and sodium 
amide are given by rCraus, 1923. 

POTASSIUM A2IDE KNg. 

SOLUBILITY OF POTASSIUM AZIDE IN WATKR. 

fttohlgcmilh, 1934.) 

The results are given in the form of a diagram but numerical values 
only for the following points. 



* 


is. KM per 


Solid 




100 M 


;s. K 3 * H g O 


Phase 




-12.9 ( Eutec. ) 




26.2 
29-3 


KN, 4 
*N, 


H 


10.5 


31-7 


ti 




15-5 


32.8 


" 




17.0 


33*2 


it 




100 


Si. a 


u 




354 'm. pt. ) 


100.0 


M 





The results at 10.5 , 15.5 and 17.0 are by Curtins and Kissom, 1898- 

100 gms. Alcohol (d t? = 0.799) dissolve 0.16 gnu KN^ at o and 0.5*1 
gm. at b. pt. 

100 ums. Alcohol (80 per cent) dissolve 1.8 gm. KN^ at o and 5.9 gm. 
at b. pt. 

100 gms. Benzene dissolve 0.15 gm. KN at b. pt. 

(Cranston and Livingstone, 1926.) 

POTASSIUM NITRITE KNO* 

SOLUBILITY IN WATER. 

(Oswald, 1912, 1914.) 



Gms. KNQ} 
t*. per 100 Gms. 
Sat. Sol. 


Solid ^ 
Phase. l ' 


Gm. KNO, 
per xoo Gnu. 

Sat. Sol. 


Solid 

Phmst. 


4.1 


16.1 


Ice +I7-S 


74-5* 


KKOb 


- 7-6 


24.1 


25 


75-75 


M 


13.8 


40.2 


40 


77 


< 


-18.6 


50.1 


55 


77-S 


4 


24.6 


61.7 


75 


78.5 


14 


-30 


69.8 


100 


80. s 


41 


31 .6 Eutec. 


71.8 


" -f KNOa 1 1 1 


80.7 


4* 


6.5 


73 - 2 


KNOa I r (; 


81.15 


4 


o 


73-6 


125 


Hi. 8 


44 



roc gms. H 2 dissolve about 300 gms. KNOj at 15.5, {Div^r-4, i 

The figure 138.5 gms. KNO 2 ^r ICK> gnw. H a () at 15, given by von Niemen- 
towski and von Roszkowski (1897), is evidently low. 



KALIUM . 832 

POTASSIUM NITHITE KNO p . 



OF POTASSIUM NlTRITt IN WATER. 
(Bureau. 



Solid 



Ice 



"12.25 
-20.4$ 

-40.2 (Kutec. ) 

-26.8 



27.85 

41*0 

64.9 
68.it 



d.or <*. wo ? i 

1 sat. aol. 100 *. **t< 

-8.9Ur.pt.) 71.9 

+20.0 1.6n9 7U3 

56.0 1.671 76,36 

64,7 1.673 77.0 

79.5 1,687 7H.5 

98.5 1.71U 7B.<> 



KNO 



40 



. ptr 100 

MC. SOI. 

73.65 
75 ^ l 

77.00 
77.75 

78.98 
80.35 



The above results for th* ice curve iliffer frc^m ihcn^ of Oswald, 1912, 
i9m- They also show the ^xistcjnc^ of the hydrate, KNO f .<H f O. The 
results between o anil 98 Are by fUkow.sk i ad Sl^wina, 10*^1. These 
authors also give renultn for the Ice curve* which *i|frw with those of 
Oswald, 1913, 



SOLUHILITY or POTASSIUM Hirtxti IH Auuioys SOLUTXOHS or 

POTASSIUM HITIATI AHO VICE VBXSA. 



Results in the form of a diAgr^w are presented for the temperatures, 

o 25, 56. 6 g and 98.5 but numeric*! values are given only for the 

temperatures 25 and 98. $^ 



Results at as 



Result * At 96.5 



fas. pr 100 



f 


"^^T~^ 


68.7 


8. S3 


66 . <i s 


n. ao 


64.15 


13.05 


6us 


15-10 


SS-8 


14.95 


35.85 


15.05 


19.90 


18.75 



MC, 



in ,80 
n.8o 

1$. 15 



19.70 

30.ni 



MC, KNO^ + KNO = Mixed CrystAls. Dm* for ihU syste at o , 30, 
^o, 60 '8o an 8 98 Are also given by fUkowsky md SlavinA,, 19^1, b 
the results are not in good accord with the 



but 



833 KALIUM 

POTASSIUM Cobalti NITKITE K 3 Co(N0 2 )o. 

SOLUBILITY OF POTASSIUM COBALTI NITRITE IN AQUEOUS ALCOHOL AT li. 

(Picrrat, 192 1/) 

NOTE. Saturation was obtained by agitation for several hours. The saturated 

solution was evaporated to dryness in a current of air and enough water to yield 
the original volume of the solution was added. The nitrite in this solution then 
determined by calculations from the electrolytic conductivity. 

Wt. per cent C S H S OH Gms. K,Co(NO^ Wt. per cent C,n s OH. (Jras, K 3 Co (NO^ 
in solvent. pe,r liter Kttt. sol. In solvent. por liter sat. ol. 

o.o 0.21 27.3 o.o36 

8.7 0.09 4 a 4 o.o33 

1 5. 7 o.o56 94-7 o.ov.6 

Data for the fusion-points of mixtures of KN0 2 + KN0 3 are given by 
Meneghini, 1912, and for mixtures of KNO g + NaNO p by Rttinger, 1932- 

POTASSIUM NITRATE 

SOLUBILITY IN WATER. 

(Mulder; Anclrac, 1884; Gcrardin, 1865; Etard, 1894; Ost, 1878; at 31.23, K5hkr, 1897; Kulw, 1904; 

Tildcn and Shenstonc, 1884; Berkeley, 1904.) 
Average Curve. 

Gms. KNOa per 100 Gms. Gms.^KNOa rjer 100 Gma. 

* " Waten Solution. " Water. Solutknau 

o 13.3 ii. 7 70 138 58.0 

10 20-9 17*3 80 169 62.8 

2O 3I-6 24.0 9O 2O2 66.9 

25 37.3 27.2 IOQ 246 7I.I 

30 45 - 8 3*-4 no 300 75.0 

40 63.9 39.0 120 394 79 - 8 

50 85.5 44-o 125 493 8 3-* 

60 no.o 52.0 



The very carefully determined figures of Berkeley are as follown: 





r/,of 


Gms. KNOa j>er 


t 3 


<LoC 


Gmn, KN'O, ji 


t. 


Sat. Sol. 


100 Gms. Hj,O. 




Sat. Sol. 


too Omn. H'J( 


0.40 


I .0817 


13-43 


60.05 


^3903 


in.xH 


14.90 


1.1389 


25.78 


76 


1.4700 


156,61: 


30.80 


I .22l8 


47- S 2 


91.65 


i -5394 


21:0.20 


44-75 


I-3043 


74-5 


114 b, pt. 


i ,6269 


311.64 



IOOO gms. H0 dissolve 384.48 gms, KNOa at 25. (Armstrong and Kyre, i^iO-u.) 
One liter sat. solution in water contains 2.8 inuls. 283.11 gnw, KN() 3 at 20. 

(KoHenhtnm and Wcinhclcr, i*to u I 

Recent determinations of the solubility of potassium nitrate in water, ugrcn'ing 
satisfactorily with the above data, are given by (luigaev and Khlopin (|<>14K 



KALIUM 834 

SOLUBILITY OF POTASSIUM NITRATE IN WATKR. 

Determination at temperatures up to 60 made by Massink, 1917-18; 
Gladstone and Saunders, 1923; Wright, 1937; Maljuori, 1928; Nikolajew, 
1929; Benrath and Wazelle, 1929; Bhret, 1932; MuUer, 1933; Ricci, 1934 ; 
and Saslowsky and Ettinger, 1935; imcl for temperatures above iocf by 
Rrdnsted, 1913; Aronowa and Lumskaja, 1931 and Benrath, Gjertebo, Schiffers 
and Wunderlich, 1937, were plotted and the following values taken from 
thA avovitff /-nrvA HrAwn through them. 



the average curve drawn through them. 



o * a * K*O S per 

100 &* At. soi. ** 100 !* U ol. 100 PIS. flat. aol. 

. ) 10.87 ^o 5^-S 180 87.0 

12.2 70 S7S 300 89,0 

K> 17.S SO 62.$ 32$ 91.7 

20 24.0 90 67O 250 93.5 

25 27.5 100 7UO 275 96.0 

30 31.2 *30 77*5 300 98.0 

40 38.0 HO 81,5 336(ra.pt.) loo. o 

50 45.S *6o 85.0 

POTASSIUM NITRAT1 KNO* 

SOLUBILITY ICE CURVE AND SUPKKSOLUBILITY ICE CURVE, 

I, 1908.) 

Ctma. | KN(>| ..... pcr_ioo Cms. Btf). 

SotuhtUty Hupersolubflity 

Ice Curve. Ice Curve. 
S-762 
S.694 
XX. 12 
11.82 

SOLUBILITY OP POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC 

ACID AT O u . 
(Bagel Compc. n&d. 104, 913, *ST..) 

Sp. Gr. of Equivalent* per so cc. Sc4uti<m. Gram* fit 100 cr. Solutlcn. 



l< 

of Cryst. 


' Solubility 

Ice Curve. 


SupenolubUity 

Ice Curve. 


of Cryst, 


I 


3-336 


I. Oil 


-3 


2 


7-SW 


3-53 


-.4 


-2.8* 


ii, 6a 


5.56 


-s . 








-5^3* 


* Cryobytifftte. 



^ HN 65 

9.9 " 5.87 " 10.02 l4 3.71 " 

.093 8.28 " 13.2 4I 8.38 " 8,38 

"7 7-4 " 21.55 " 7 '49 <4 13 -S 8 " 

.144 7.4 " 31.1 " 7,49 ** 19,47 *' 

.202 7.6 " 48-0 '* 7-68 4< 30.04 " 

,289 10.3 " 68.0 M 10,42 * 4 42^86 f< 

1.498 28,3 xao.s " a8.6 4 4I 75.95 <f 

Fr^adng-point data for KNOi 4- HNOi are given by Dernby (1918). 

SOLUBILITY OF POTASSIUM NITRATK IN AQUI-.OI-N Soi,irr$t,\*4 ot-- Nrnut; ACID 



Per cm HJiOj Gm. K.XO, Pwrri{%<l s (; ffl . K\0 a lrr rnil HN< 4 l.m*. KNO, 

In Mlre-nL por lOOgm*. Mlveitt. In ohtti. jttir tgi *<>hPMi. lit ohni. jH'r 

3 1. 4 4****> *".** 70 

lo - ^9.1 S<i iH.> H^ 

ao-o i4-5 Cm it). li c|i 
3o . o n . 4 



835 



KAIIUM K 



SOLUBILITY OP POTASSIUM NITRATR IN AQUEOUS SOLUTIONS 

OP NITRIC ACID AT 25. 

(Mai quo rl 19P8C.) 



(tea. pr 100 agas. aat. aol. 



Ctea. per 100 gaa. a at. aol. 



0.00 

10.30 
13*97 

20.11 



27.31 
25.03 

24. 13 
26.12 



29.56 

44-17 
50.01 



35^0 
43*28 
49-99 



SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC ACID 
AT SEVERAL TEMPERATURES. (Kuxantxov, 'i923, 1925.) 

Constant agitation was employed 1'or securing saturation. One to two hours 
was found sufficient in all cases for the attainment of equilibrium. 



Results at 0. 

Cms. per 100 gins, 
sat. sol. 


Results at i;>. 

Cms. per 100 gins. 

KUt. SOl. 


Results at ;). 

dms. per 100 gnis. 
sat, sol. 


Results at 75. 

<;ns, per 100 |m%. 

Mil. M>l, 


KNOT* 


i . ' ^ 

KXOj. 


HNO,. 


I < 

KNO 


a> 


HXO,. 


_'S MM "-" 

KNO.,. 


HN() a . " - 


*>"- 





.O 


II 


9 




0.0 


20. 


7 


O.O 


'*!.> 


O.O 


<>(>.<> 


I 


.3 


II 


.0 




7 .5 


14- 


2 


5.4 


2 .'5 .6 


r >. I 


53.6 


4 


7 


8 


.5 




18.0 


10. 


7 


I I .0 


'>.(), f) 


17.7 


4 1 . :j 


8.7 


7 


.2 




23.3 


IO. 


i 


18.1 


I7.V, 


21. H 


38. <) 


i3 


.2 


6 


4 




24.0 


10. 


2 


^.7 . 2 




'>,<) . 3 


37 . 4 


16 


.5 


6 


. i 




29.2 


IO. 


5 


4O. I 


f, 8 . <) 


3u . u 


36.7 


25 


.5 


6 


4 




4o.o 


i3. 


6 


47-7 


27. 7 


38. r > 


37,6 


3o 


.1 


7 


.0 




45.i 


*7- 


7 


49.0 


33. v, 


42.5 


39-9 


33 


i5 


7 


.5 




49-3 


25, 


i 


So. i 


3 9 . > 


45.5 


43.<j 


39 


9 


9 


7 




5i.o 


3 2 . 


7 


5o.6 


42.5 


46.7 


So . o 


48 


.0 


16 


.5 




5i.6 


38. 


i 


49*7 


49-9 


46. a 


ft 2. 


5o 


7 


23 


. i 




5 1 .3 


44- 


i 










52 


.2 


3o 


.2 




5o.o 


49. 


2 










52 


.2 


38 


.2 


















52 


.2 


39 


.4 


















5o 


7 


48 


4 


















57 




34 


.4 


(Soli 


d Phase = KNO.H.^HNOa) 


73 


.0 


25 


.5 


( 










) 








SOLUBILITY OF POTASSIUM NITKATE IN AQUEOUS SOLUTIONS OF 
PoTAssiuk HYDROXIDE AT !M). (Bri>ntod, 19*0 o). 


Cm. mots. 

"i^fc ^^ 


per liter 

***tf**~~~~~" 




Gtu 


. mob. 


per liter 


<;m, uu>l 


*. per liur 








KOH. 




KN0 3 . 




Ttoif 


""""^X 14 * 


KNO|7* 


'K<MlT**^ 


KN0,. 








4.71 


0.847 9-4* 


0.364 


l.-j.OV. 


0.v.4l 








7.90 


0.455 


10.95 


0.298 


14.85 


, 232 








7-95 


o.45o" 


12. 19 


0.27* 


1 5 . 02 







KALIUM 



836 



SOLUBILITY OF POTASSIUM NITRATB AND OF ACID POTASSIUM 

IN NITRIC ACID. 

(Grotchuft --* Bcr. 37, 14^0* *O4.) 

NOTE. Determinations made by the so-called thcrmornetric 
method, i.e., by observing the temperature of the disappearance of 
the separated, finely divided solid from solutions of knc vn concen 
tration. 



Grams per 100 Cms. c ... 
t .Solution. gjfid 


Gm. .per 100 Cms. 


Solid 


JCNOt. HNOi. 


f^hT^Jim^, 


I*hase. 


- 6 24.4 75.41 KNO.HNO <) 


2^,5 47.2 52.93 


KNOj.HNOa 


-f-14 3 2 -^ 67.42 ** (ftUbll) 


3 3 S 47 -8 52.11 


M (Mbll) 


17 34.8 65.04 


3 S-S 4^-6 5^4<^ 


M 


19.5 37.2 62.90 


-^70 40-4 50 7H 





22 44-5 SS'46 


.'0 5 ! 40 04 


KNOaHNOa 


21.5 47.8 52.11 XNO|.aHNOt( : > 

21.5, 48.6 51.46 " CUWD 


30 5 50-0 40-15 

Ji o 40-4 50.78 


(bbil) 
^^k (Ubil) 


20 50.9 49.15 
4 37-2 62.8l KNO|.HNO| 


3^.0 50.0 40>5 
50 51.7 48.32 


4t (ittbU) 


-16.5 44,5 55,46 " <Ubi!) 






( l ) Solution in HNO|. 


I 1 ) Knluiinn in KNOi. 




CONDUCT OP ACID POTASSIUM 


NlTRATH TOWAKDH WATER* 


Grrw. per roo Cms, . 

**' r--J^i!fl-^ * 


f <5m% 'jis r ttifc;. <imii 


Solid 


22 44.5 55,5 KNCJi.)HNOi 


50 3 7 4 .1 


KN^ 


20-5 44.1 55.0 


6 1 36 o 44 8 


* 


18 43 -8 54.5 


63 34 ; 4|. 





12 43,0 53.6 


60 5 30 g 39.5 


M 


6 42.3 52.7 


56 *7^ 34-4 


** 


o 41.6 51.8 " 


43 20 8 25.9 


N 


12 41.3 51.4 KNOi 


17 tt 7 14.6 


+* 


22 40.9 51,0 


-5 5-54 6,91 


44 


40 39-9 49.8 " 







SOLUBILITY OF MIXTURES op POTASSIUM NITRATE AND POTASSIUM 
CfiLOKznB IN WATKK. 

(Etard - Ana. c 



Gmf.jper too Cms, 



Cms. per too Gmn. 



_ pwL M 



Omn. |rr too CBMU 





KNOi. 


KCl." 


KNf 


i,/ 


"TR 


T 


m 


g~=- 


no? 


O 


S-o 


20 


O 


30 


1 6 





81 


-2 


70 


39 5 


17 .5 


ro 


.0 


20. 


,8 


40 


Ji 


o 


ai 





80 


45 5 


15.8 


20 


12.6 


21 


-2 


50 


*7 


(3 


20 


O 


100 


57 5 


n 6 


2 S 


14.0 


21 , 


'3 


60 


33 


S 


19 


,Q 


120 


69 o 


7-7 



837 KALIUH 

POTASSIUM NITRATE 

EQUILIBRIUM IN THE SYSTEM POTASSIUM OXIDK, NITROGEN 
TRIOXIDB AND WATER AT 25. 

(Nlfcolajew, 1928.) 

Acid Branch Alkaline Branch 

Otas. per 100 BBS. oat. aol. Solid One, per 100 ^a. nat. aol. Solid 



f HNO KNO^ v Phaao f" KOJ? KNO~ x Phaa 

o.o 27.87 KN0 3 5.11 20.36 KN0 3 

9.89 19-00 " 12.25 13.31 " 

16.68 15*27 " 17-38 9/59 " 

32.29 14.02 " 29*6$ *-<5o " 

42.57 17.15 " 39.82 2.49 

49.53 25.37 " '19.79 114 

50.85 1.05 " * KOH 

54. 18 o.o KOH 

This author also gives results far equilibrium in the system KNO + 
NaN0 3 HN0 3 * H ? at 25. 

SOLUBILITY OK POTASSIUM NITRATE IN AQUEOUS SOLUTIONS 
OF HYDROGEN PEROXIDE AT 25. 

(AKtrlof and Turck, 1935.) 

Wt. Percent H p Ou On. Mola. KNO_ Pr 

In Aq. Solvent 1000 9*8. Solvent 

0.0 3-774 

15.72 4710 

31-43 5.762 



SOLUBILITY OP POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF: 

(Touren Compt. rend- 13 1 350, 'oo.) 

Potassium Carbonate. Potassium Bi Carbonate. 

Results at 14.5*. Results at 14-5** 

Mols. per Liter Gms. per Liter. Mol*. jyr Liter. 

KsCOa KNOa. * KaCOa. KN0 3 - fcHCO|V KNOi 



o-o 2.228 o.o 225 o.o 2.33 o.o 236 

0.48 1.85 66.4 188 0.39 2.17 39 .o 220 

1.25 1.39 172.9 141 0.76 2.03 76.0 205 

2.58 0.86 356 .9 87 1.16 1.92 1 16 i)4 

3.94 0.64 544-9 65 1.55 i. 81 155 183 

Results at a$. Results at s : ft 

o-o 3-217 o.o 326 o-o 3-^8 o o 332 

o 59 2.62 81.6 265 0.89 2.84 89 287 

135 1.97 186.7 *99 i-33 2 ' 6 5 ! 33 **& 

210 1.46 290.5 148 1.91 2.45 igi 249 

2.70 1.14 373.6 115 

3.58 0.79 495.1 80 



K KALIUM 83 

SOLUBILITY OF POTASSIUM NITRATK IN* AQUEOUS SOLUTIONS OF POTASSIUM 
CARBONATE AT 24.2. * 

(Krfrairtrt ami /itrk, p;toy.J 

Cms, per logo Oms._HA_ Solid jSl!IilI!ILi2S^ Solid 

* KNO a . ' i^T !')* KM),. K^TST 1 Phtse. 

376.8 o KNOb 73 688.1 

285 130-3 " J 8 - 8 8 ? 8 -3 

161.7 348.4 " 3 1 - 1 012,2 

141.8 371.9 

1000 gms, H0 containing i tnol KC1 (IOI.M gnw.) dtwiolvr 324,85 gm t KN0 8 

at 25. < Armrong and Eyre, xgio-xi.) 

Data for the system potasatum nitrate, |M:>lai*.iii u!fat(% water at 35 are 

given by Massink (1916, 1917), 



SOLUBILITY OF POTASSIUM NITRATI- iw A^t'^ot'H Sou MONM tn- PUTAHKIUM SULFATE 
XTA AN VICK VKHSA AT SS<.VI:UAS. I'l MrrwATiiiiim, 

W(J (luimyr, If2, M ' ' 

(iiiw, jwr IM gmi. 

Ml. It>l. 

t". KXO,, K } S< 4 , Sttlitl IMi.M*- t R:^IS I K,H>, jjiilld Phase, 

?,5... 217. (>4 o.o (I) K\o, 




ri... 76.01 1,98(1!) 

',>, r >. . . u't*99 44 ; ^ H 1 

.'> ... i { . '>ys 5 %Hf| ( I ) HI w>, 

u5... n.ol G.KJM'.tl) i iti,,, ri.ip *JVI|II) W4-BXO, 

^100 gms, lolution timtltatii k ouitty Muttiratrtl with |t<ttttium nitrate and sodium 

nitrate contain /$5'iC> K NC* a 1- '^7' r *7 K l|ls - i * S| ' 11 ^** |kt *)'* f Humid, iw.i 

Data for the qutrtemary ytt*i!i K Nci 3 ? KjSO, * NH No., * N% S(,) 4 *-|- H 
at a5 and at 90 arc* given by Hamiil, iyjf, ' ' * 



OF MIXTURES op PoTAnsnrM NITRATE AJJW PotASSitni 

SlIlWIATK IK WATtfR, 
(Pvlrr -7. filtyiik i h. 4 Hi* V4 ) 
t*. Sp* Of. *4 St. fcitiiffon, fir tr |^r tw Crv* XV^irf 

15 1-165 24 1j KKU i 5 61; k Sf> 4 

20 ... 30.10 H 558 '" 

a$ X. 210 36,0 * 4 5.58 " 



839 KALIUM 



POTASSIUM NITRATE 



SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS 
OP POTASSIUM SULPATK AND VICE VERSA. 

(Herlng, I9?fl, 19?7.) 



d. of Oms. per 100 i8. H.,0 Solid 


d. or Ctas. per 100 gms. H &>J 


sat. sol. ' KN0 3 


K,>SO x Phase 


sat. sol. /"" KNO ? """" ^"^ 


V* J 4 


rfH 


Results at -3. 


32 (Eutec) 


Results at 


40 




10.3 


11.7 Ice*KNO ? +K p 


SO^ 1.787 61.0 


5 . 00 


KN<V 


Results at o 




Results at 


50 




13.3 


o.o KNO, 


1.339 83.3 


3.20 


KNO S 


12.0. 


3.<6 " " 


1.341 82.5 


4.53 


" * 


12.2 


4.95 " + K ' ? SQ 4 


1.301 68.7 


4 54 


K^Sl') 


1 1.0 


5.05 K p S0 4 


1.203 34.9 


7.9 




6. a 


5.74 " 


1.171 24.9 


9.2 


*" 


0.0 


7.33 " 


1.152 l8.0 


10.6 


M 






1.104 0.0 


16.5 


" 


Result at 8,5 















Results at 


75 




18.1 


S...5 KNO^S), 












1.467 150.5 


3 * \ 


KNO 


Result at 1*7. 


5 


1.433 131.2 


3*71 


K ? SO 






1,380 105. S 


4 . , \ 


11 


1.176 22.7 


5.77 KNO^-fK 80 


1.335 86. j 


5.18 


" 






1.268 6o.r> 


7.01 


) 


Result at 20 




1.197 39.1 


9.75 


" 






1.148 17. a 


M.H 


" 


1.187 3.0 


5.71 KNVK,S\ 


1.116 o.o 


;>o . 6 


" 


Results at 25 





Results xt 


100 




37.3 


o.o KNO, 


1.572 242, 


2.85 


KNO 


1.205 36* y 


4.67 " ' 


1.566 237 3 


2.75 


p' 


1.210 35.7 


5.86 " + K ? S0 4 


1.567 337.4 


2. Ho 





1.199 32.4 


6.06 K^SO 


1.497 182.0 


3.49 


i 


1.170 25.0 


6 . 78 " 


1.467 162.3 


3.31 


H 


1.144 l8.0 


7.78 " 


1.394 120.6 


4.8*; 


II 


1.115 10.3 


9.09 " 


1.35.1 i oi.o 


5.60 


Jl 


1.086 


12.10 " 


1.229 50.4 


9-46 


tl 






1. 163 25. 3 


14.0 


H 


Result at 30 




1.119 0.0 


74. I 






K KALIUM 



POTASSIUM NITRATE 



SOLUBILITY or POTASSIUM TITRATE IN AUHBOVS SOLUTIONS 
OF POTASSIUM SOLFATR AMD VICE 



The results are expressed in terms of number of gram molecules of H 
required to dissolve 100 f*m. mols. of salt or salt mixture of determined 
mo I ecu 1 ar composi lion. 



Hoi. 


* KNO, 


toi. HoiS. H,,0 U) 


Hal. WO^ to. Holt. H p O w 


in dlsaolvta 


aiMOlvt too P 


in diniwlvttt ai^wiv* JCK) pit. ^ ll<1 


salt 


mixture n 


iols HAH MiKtur* * 


MUMUCUM WU. MllAlXCUrt PhMi 




Results At 





He*Hult.H At 2<^ (con.) 







118* K SO 


Ho 250 K SO 




20 


975 ?n * 


?5 3<H " * bo 




uo 


750 " 


ioo 370 KNO^ s 




60 


S10 " 


V 




64 


520 " * KKf 


) Kr*Hu! tn ill 50 




80 


6v> KNO, 






100 


760 


o ^28 ^^^ 4 




Results at 


as 


*|O Y7Q H 








60 aHo " 







72^. K f Sf) 


80 190 " 




20 


625 


>< no " * KNO S 




40 


520 ** 


itx> 11 a KNO^ 



60 



Results are also given for the reciprocal n*i i p.Air KK'C)^ * IN 
: ? 80 4 * 2NH 4 NO S . 

EQUILIBRIUM IN SVSTIHS OnHpntttft nr FIITASSIIIH AMI SODIUM 

NlTXATIta M". 



Complete experimenidl dai* f incltitiing dmiti f ia the form of tabular 

results and diagrams for these comi>i*x sysienM *i i|*ef^ttires between o 
and 90 are given by Corner, and KreMnb4ch i^j*i Aid Oirnec, Knwbach and 
Spack, 1930. These Authors have mvU UHI* whf never nec^HHAry of the re- 
sults for the ternary systww tnt |ii4ier#iry Hy.*fie pnrvtouHly reported 
from their own UborAtory or by others, ificitttliitg Chreiien, 1939; Cornec 
and Bering, 1925-7; Corvee MC! Kromb*%ch v 19.19; Hryerhoffer 4fl4 Sounders, 
1899; O'Ans, 1915 and BlaAcUle, 19 1, 



SOLUBILITY OP POTASSIUM NITRATE IN AQUKOUS SOLUTIONS 
OP MAGNESIUM NITRATE AND VICE VRRSA. 

(Benrath and Benrath, WPgfa), 1930J Benrath and Slchelschraldt, mi.) 



KALIUM K 



d. of 
sac. sol. 



1.079 
1.091 
1.106 
1.146 

1.296 
1.350 
1.389 
1.382 
1.369 



1.194 

1.202 

1.221 

265 

320 

438 

462 

431 

394 



,318 
.316 
.361 
.455 

459 

SOS 
.462 

1.416 



1.470 



445 
432 
426 
510 



1.510 



645 
1.599 
1-537 
1.461 



1.529 
1.532 

1.555 
1.672 
1.690 



One. per 100 m&. sac. sol. 



'Mg(N0 3 ) 2 


KNO.J' 


Results at 





0.0 


11.7 


2.26 


11.5 


5- '15 


8.35 


11.06 


6.48 


17-55 


4.29 


27.29 


4-35 


33*42 


4.40 


37.6 


3.26 


38.45 


1.09 


38.58 


0.0 


Results at 


25 


0.0 


27. M9 


5-98 


21.40 


10.06 


17.84 


18.73 


12.41 


26.09 


10.18 


37.2 


8.63 


39.3 


7.67 


40.49 


3-OB 


42.0 


0.0 


Results at 


so 


0.0 


46.10 


4 . 44 


39.37 


14.12 


28.36 


26.18 


19.36 


35-86 


15.45 


37.03 


15.40 


40.47 


15.02 


42.50 


8.32 


45*44 


0.0 


Results at 


75 


0.0 


60-53 


3-78 


54.17 


13.52 


40.68 


23.30 


30.76 


34.07 


24*04 


40.41 


22.30 


44.58 


22,00 


45.69 


16.96 


48.01 


10.15 


51.00 


0.0 


Results at 


99.5 


0.0 


70.8 


12. 14 


54.52 


23.19 


42.90 


37-93 


32.05 


38.46 


30.93 



Solid 
Phaa 



MglNO 



.6H g O 



KNO. 



NO 



KNO,, 



KNO, 



" * Mg(NO I .6H 



MgNOj|) f .6HfO 



KNO, 



Results are also given for the reciprocal salt pair <KN<V t 



K KALSUM 

SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS 

OF AMMOHIA AT o. 
(Ouyr Bltitr ana Hctwid* 19^4.) 

The authors present their results in the form ol diagrams hut do 
not give their experimental determinations. The following approximate 
values have been estimated from the published digram. 

<k. or 100 t. MC. tol. lld nM._ _ ptr 100 y. MC. ML. Solid 

fo 



NHj, 


KNO, 1 p ^^ 






0.0 


12,0 K'K0 3 


10*0 


8.0 w 


20.0 


S*o " 


30.0 


U : 


50.0 


7.0 




SOLUBILITY or POTASSI 



ITIATF i^ LIQUID AHMOKIA. 

t ; Auaof|w 

1 8&U Ml. '^MU Ml. *M, ^ 

Q.O 9.52 to*S2 U*inhird dnt Stephnn, 191^. 

o'.i 0.695 9-7 l * 7li (SchAtlenHtein AIMS Monosohn f 1932.) 



TUP SYSTEM AMMONIUM Nrr4*ri; I- l*or*HHiuM NiTtt\tn 4- WATER AT'B, 

! AfHl*i i!J,, f 

Saturation was obtained by conitanUnt rotation in a thrmotat. The salts 
form two series of solid nolutiam with n gap. 

Jim*, pi-r 100 m 

KXOj. Hull*? lH%r. ^ $ ^ s KM I 8iiU<l fhw. 



o.o 



G:l.G3 a.;i 

61 41 7 ;.(> 

5t),q3 H.Gi 

5^,80 18.95 



Solid solutions of 




KNO4-NH t NOt 



NHiNOjstturatcd i<hi> *7 | Solid solutions of 

wilhKNOi v. r MV *n.:iH KNO :| saturated 

with NH 4 NO 



Similar, but apparently les nccuratt results* dattrmmad at th ordinary tempe* 
raturo, aro given by Caiitftrt, 1918* 



Very complete data for ihf ct^pl^x riy^tcw KNO * NH NO, * H f O, in which 
several modifications of ihe mix crystal H fiiul HttutioAH) of iht two 
salts are formed, are given by Jiineckc, s^aH, Anil v*ry much more complete 
results by Jftnecke, Hin<icher and KAhlfn, 1*1^3. Th^-i* Autitors n^if wor^ 
thau\ 300 solubility detf-rwinAiiofti r inciudinir 4nAlys**s of IwHh ihr HAtu- 
rated solutionn and solid phases. Tin* rttiliH *re fn* s $^nti io iht form 
of tables of experiment M deterfnift*iii4ifln A&I! (ttA^r^ns which nhow the 
limits of composition and field* of *Ki%i*tce of i**icti of the several 
modifications of the wix crystals AS wtll an th? corresponding composi- 
tions of the saturated solution* at temper At ur<* lietwe^n -i*; And 

Data for the mix crystiils, solutions t)ri nlt$t io the Syntiw tK t 
(C1,N % 5 ) are given by Jtneck*, 1938.) 



843 KALIUM 

SOLUBILITY OF AMMONIUM AND POTASSIUM NITRATES AND SULFATES 
IN WATER AT 25. (Osaka and inouyo, 1925. ) 

Mixtures of the salts in roughly calculated proportions were rotated in a thermostat 
for several days, and both the saturated solutions and the solid phases were ana- 
lyzed. There are five scries of solid solutions present as solid phases. These arc 
1. (NH 4 , K) S SO*; 2. (NH 4l K),(NO,) 2 a; 3. (NH 4 , K) a (N0 3 ; t p; 
4. (NH*, K) 2 o.5SO 4 o.5(i\'Oa)j; 5. (NIi t7 K),o.4 SO*o.C>(N0 3 )*. 

Complete tables showing the composition of the liquid and solid phases for each 
of the five scries of solid solutions are giyen. The results are presented in gram 
percentages, and in racial proportion according to the formula 



K 



SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND SODIUM 
CHLORIDE IN WATER. 

(Etard Ann. chim. phys.JYJ 3, 383, '94; the older determinations of RQdorff, Karaten, Mulder, etc, 
agree well with those of Etard.) 



Gms. per TOO Gms. 
t. Solution. t. 


Gms. per TOO Gms. 

Solution. t. 


Gms. per too Gms. 
Solution. 




ICNOa. 


NaCl. * 




'KNOa. 


NaCl.' 


iCNOi. NaCL 





13 


24 


40 


30-5 


19 


1 20 


73 




8 


.0 


IO 


16 


23 


50 


36 




140 


77 




7 


.0 


20 


2O 


22 


60 


42.5 


3C S 


160 


79 


5 


6 


o 


25 


23 


21-5 


80 


55 


12 


170 


80 


5 


5 


S 


30 


2 5 


20.5 


100 


67 


9-5 













NO 



loo gins; HA simultaneously sat. with potassium nitrate and sodium chb- 



UC, CUllLd 

- 39-81 g: 
SOLUBI 

Sp. Gr. 
Sat. Sol. 


LIU 4.1.14 gms. iv IN 
ms. NaCl at 80. 

LITY OF POTASSIU 
CHLORIDE AND 

Results at 20. 

Gms. per loo Grm. HaO. 


us -r 30.53 gms. iNav. 

M NITRATE IN AQUE 
VICE VERSA. (Leath 

Solid Sp. Gr, 
Phase, Sat. Sol. 


.1 at 25- ana 105.5 ] 
ous SOLUTIONS OF 

ier a&d Mukerji, 1913.) 

Results at 30*. 

Gms. per xoo Gmt. K|O. 


gms. J^lNOu 
(Soch, iH<$.) 

SODIUM 

Solid 


KNO a . 


NaCl, 


1 KNO. NaCl.^ P*w. 


1.167 


31-49 







KNOa 


I 


.261 


46. 


48 


9 


.82 


KNOi 


I.22O 


33.41 


9- 


94 


" 


I 


.302 


47. 


08 


20 


.18 


44 


1.267 


34-93 


19. 


44 


" 


I 


343 


47- 


24 


29 


.86 


a 


I.3II 


36.41 


29- 


46 


" 


I 


372 


49 * 


24 


38 


.72 


M 4-NnCl 


1.344 


37-30 


37- 


73 


" 4-NaCl 


I 


342 


33. 


36. 


38 


55 


Nad 


1.330 


31.41 


37- 


57 


NaCl 


I 


.298 


25- 


32 


38 


23 





1.283 


19.56 


37- 


51 





I 


.258 


12. 


15 


37 


38 


< 


1-243 


9.76 


36. 


73 


" 


I 


.202 






36 


30 


M 


Results at 


40*. 


Results at 


91. 




1.288 


64.74 


o 




KNO, 


1 


552 


2O2. 


8 


o 




KNO, 


1.320 


64.66 


II. 


32 


" 


I 


573 


204. 


2 


12 


.Si 






64.05 


23. 


41 


tt 


I 


.601 


208. 


I 


28 


45 


* 


1.396 


64.13 


35.08 


I 


645 


2X3- 


3 


37 


.Q2 


tt 


1.411 


64.77 


38. 


79 


" + NaCl 


I 


.660 


2*8, 


8 


39 


.08 


< l 4-NaCl 


1.376 


52.8l 


39. 


51 


NaCl 


I 


.607 


175. 


8 


40 


,8 7 


NtCl 


1-323 


34.98 


38. 


98 


" 


I 


5^7 


126. 


9 


44, 


33 


u 


1.267 

A 4. il__ l_: 


17.33 


37. 


74 


" 


I 


.378 


57- 


53 


42, 


,C)0 


' 



At the higher temperatures, results for NaNO a in certain solutions are reported. 



KALIUM 

SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS 
NITRATE AND VICE VERSA. (leather and 



SOLUTIONS OF SODIUM 
Mukerji, 1913.) 



Results at 30. 

Gms i>cr too Cms. 
Sp. Gr. HO. 


Results at 40. 

^ Cms. IKT 100 Gm*. 
Sp. Gr, HA 

J^k t^j -?' 


Sp. Gr. 
Sat. &t>l. 


Results at 91. 

Gnu. per loo Cms. Solid Phase 

|U. ; n 


Sat. Sol. 


KNOa. 


NaNO,. 




KNO a , 


NaNO* 




KNO* 


NaNO a , 


. Each Case. 


I.3I7 


45-73 


25.90 


1.358 


63.21 


23.85 


1.615 


200.8 


43-4 


KNO, 


1.403 


47-25 


52.53 


1.428 


63.86 


49-79 


1.674 


207.2 


Q2.QC 


> " 


1.472 


50-93 


79.27 


I.50S 


66.44 


79,46 


1-75* 


229.5 


156.2 





1-544 


54-34 


1034 


1.570 


74.06 


1x6.2 


1.700 


251.8 


206.5 


" 4-NaNO, 


1,520 


47-67 


I03.I 


1-573 


68.72 


116.7 


1.774 


2II.7 


2OO 


NaNO, 


1.481 


30-25 


101,6 


1.526 


43-92 


112. 2 


x. 605 


128.5 


xS6 




1.451 


14-30 


99.10 


1.476 


20.33 


IOQ.Q 


i.6to 


55-75 


173.1 


<i 


1.406 


o 


95-90 


1.421 


O 


105.2 


1.521 


O 


160.8 


" 


Results at 20 


are also 


given. 















SOLUBILITY OF POTASSIUM^NITRATB IN AQUEOUS SOLUTIONS OP SODIUM 

NITRATE' AND VICE VERSA AT 20. 

CCarnelly and Thomson J. Ch. Soc, 53. 7&. *8&; NJcol Phil. Ma. 31, 360, *pi.) 

KN0 8 in Aq. NaN0 3 Solutions. NaNO 3 in Aq. KNO t Solutions. 

Grams per too Grams HfO. 



O 
10 
20 

40 
60 
So 



KNOi 
31-6 

30-S 

3 r -o 
33-o 

35 -S 
41 .o 



Gram* per roo Grnmn I 


O 


N 88 0|< 


10 


90 


20 


9 a 


2 S 


93 


30 

as 


94 
96 



SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS or SODIUM 

NITRATE AND VICE VERSA AT io AND AT 24.2. 

(Kromaiw ami Xitck, *yoi ) 

i. w , ,^, w i..^ trn &>||WphMfc 



fNaNO, 





KNQj,. 


NaNQa/ owmrw. 




KNO,, N*N0 4 , 


IO 


208.9 


o K^ 


to* 


24 l 


4^^ Q.M-3 


IO 


301.9 


848.3 


' -f-NaNOa 24 . 2 


437 1019 


IO 


O 


805 


NaNQi 


24,1 


I2J 6 QX0.6 


24,2 


377-3 


o 


KNC^ 


24,2 


o 913 


24.2 


390 


346.7 


*t 






SOLUBILITY op MXXTIIKBS or PaTAsaxtm NITRATE, SODIUM C 






AND 


SoDiim 


NXTXATB IK 


WATER. 








(Co rut c 


and K roaiUiiJf{ f 


IW9-) 


t 


d. or 
sat, sol. 


(tea. pt 


:r 100, ^ 


'-*-r 


S0I10 


^___ 


Hid 





104 


16,4 


38. f) 


19.6 


K^ 3 4 NaD f 


S 





19.7 


27*4 


44 -n 


i 




20 


- 


34.0 


24-3 


58.6 


H 




25 


1-475 


40.3 


33-5 


64.3 


l 




40 


- 


66.7 


20,8 


82.7 


N 




SO 


1-S8$ 


90.3 


19.1 


96*9 


W 




60 





119.7 


18,3 


114. i 


H 




75 


1.695 


176.0 


17.5 


145.0 


ff 




80 





200.5 


17.6 


158. i 


l 




87.5 


1.750 


241.5 


18.0 


179*5 


tl 




Iftfi 


1 . TOO 




t f\ A 


*^ a 


tt 





845 

SOLUBILITY op POTASSIUM NITRATE IN AQUEOUS SOLUTIONS 
OF SODIUM NITRATE AND VICE VBRSA. 

(Corn*c ana Kromuach, 193R9.) 



KALIUM K 



QMS. ptr 100 Jpa. aa 


,c. a 


icl. Solid d. or 


Qms. par 


100 t 


{na. sac. aol. Solid 


NaN0 3 


im^- 


~^ Phaa aau aol. ' ~~RaNQ 


S 


TWC 


3 




ast 


Results at 













Results 


at 


75 








o.o 


11 


.7 


KNO 


i 


.462 


0. 





60. 


4 


KN0 3 




39o 


10 


-4 


M .J 


NaNO,, i 


545 


18. 


7 


47. 


7 


It " 




42.3 





.0 


NaN0 3 


i 


.635 


31- 


3 


41. 


5 


H 












i 


.700 


38. 


3 


39. 


i 


II + 


NaNO., 


Results at 


25 






i 


.644 


42. 


4 


30. 


9 


NaNO, 












i 


.568 


49. 





18. 





i 




o.o 


27 


.7 


KN0 5 


i 


.469 


<8. 


7 


0. 





" 




40.3 


19 


. 1 


" + 


NaN0 3 
















M7-9 





.0 


NaNO, 

o 






Results 


at 


87.5 








Results at 


50 








~~ 


0. 





66. 


2 


KNO 












i 


,746 


37. 


3 


43. 


9 


" + 


NaNO, 


o.o 


46 


.2 


KNO 






6l. 


2 


0. 





NaNO s 




19.1 


35 


9 


* 


















31.7 


31 


3 


M Results at 


100 








39.8 


28 


9 


" -f 


NaNO, 
















43.3 


21 


.6 


NaNO,, 


1 


.569 


0. 





70. 


9 


KNO^ 




47.6 


12 


3 


ii 


1 


.658 


18, 


7 


57. 


7 


H 




53.2 





.0 


H 


1 


744 


29- 


7 


51. 


H 


" 












1 


.793 


36* 


7 


48. 


1 


4. 


NaNO, 


Results at 


62.5 


o 




1 


744 


41. 


1 


40. 





NaNO^ 










1 


.647 


49. 


5 


35. 


3 


i 




o.o 


S3 


.8 


KNO 


1 


507 


63- 


7 


0. 





n 




38.7 


34 


3 


" 4 


NaN0 3 
















56.4 





.0 


NaNO s 



















d. of 
sat. aol. 



1.422 

1-352 



1.189 
1.512 
1.391 



1.332 
1.434 
1.529 
1.602 
1.557 
1.502 
1.427 



1.648 



These authors also give results showing the effect of increasing 
amounts of sodium chloride upon the solubility of mixtures of potassium 
nitrate and sodium nitrate. They also give results for the quaternary 
systems composed of the chlorides, nitrates and sul fates of potassium 
and sodium at various temperatures. 

SOLUBILITY OF POTASSIUM NITRATB IN AQUEOUS SOLUTIONS 
OF SODIUM NITRATE AND VICE VERSA. 

and f.ulngtr, 1995* UK*7.) 



NO 



d. of 


Una. par 100 i 


wa. aat. aol. So] 


sat. aol. 


NaNO., 


KNOg 


^ Phi 


1. 


Results at 







1.085 


o.o 


12. 13 


KN0 3 


1.424 


39.23 


10.53 


" * 1 


1-3'|8 


42.77 


0.0 


NaNO., 




Results at 


20 





1. 162 

1.494 
1.406 



0.0 
42.03 
40.38 
46.27 



24- 13 
17.13 

16,41 

0,0 



NaNO. 



6, of 
au aol. 



3 
1.441 



1*343 



1.467 



dua. per 100 wn. ->fit, Ml. 



Results at 40 



0*0 

39.70 

51-20 



o.o 

38, 



30.00 
24 . 60 

o.o 
at 6o a 

52,0 
) 0.0 



KNO_ 



Results are also given for the <|u<tr ternary mixtures in the system com- 



posed of KNO 



NaNO, 



AUNO^). * H,0 at temperatures between o and 60. 



KALIUM 8 ^ 



Y OF MIXTIFWS OF POTASSIUM AND SODIUM NlTFATBS IN 

AQIIBOUS SOLUTIONS OF NITRIC ACID At 25 . 

. 1029.) 



Oas. pr 100 0p we. sol. Solid OM. P*r 


100 0ft*. *(. sol. 


801 ia 


'HNO., 


~ KNO,j 


Natty P&w 


if HW 3 


KNO^ NfcNO^ 


t'Jias* 



5.20 
10.66 
16.17 
21.18 


19.7 

17.68 
16.04 

i6."o6 


40.25 KNO ? 
35.26 " 
30.01 " 
23-64 " 
19.24 ** 


H ' 42.61 
" 54.04 
H 58.62 
11 63.^0 

H 


11.68 5.7S ' ' 
6.S2 4.10 
3.48 3.H2 
1,02 3.3,1 


.2HN0 3 +NaN0 3 


32.65 


16.70 


11.20 " 









OF MIXTURES or POTASSIUM AND SODIUM NITRATES IN 

OF POTASSIUM HYDROJCID* AND OF SODIUM SiYDROXTDR AT 2$ . 



Resalts for Aq. KOH ^ults for Aq. NaOH 



. . UAH.* te. Gr tOO HA*, itt. *ui. Solid 


Qfta. pr 


100 S^J^ 


ftU IMH. w 


_,,,,, 


KWO 


HaHO ** Phase 


1(OH 


KNO,, 


NSNOjj Ph 


t 






0.0 


19. 17 


^0.25 ^N0 3 * 


NaNO^ i, 17 


16.60 


38.70 KNO^ N 


1.19 


15-6$ 


41.57 " 


H Hit 


i *.8u 


3S.75 " 


2.84 
4.58 
7.35 


10.48 
6.86 

3*12 


43.00 " 
H 

42*48 w 


'* 7 * 04 

B.ao 


10* 56 

6.U7 


23,67 " 


10.54 


0.0 


40.40 H 


3i.*7 


1*J> 


7 .611 n 








40.41 


5.30 


3.14 " 



EQUILIBRIUM IN THE SYSTEM LEAD NITAATIC, I'OTAIIIIIIIM NITMATK AND WATER. 

I (Hiiistoiit* ami 8nmlr. IW3. } 



Results at 45. Rcnulw at 5IK KeMiIu at 



Gmi. per 100 fm. <t *'*" * M lll *"** ppf ?f ** Im * 

Silt, gl. 



0,0 37.17 -79 "- ''J' 1 ;? 

^. 7 5 37.37 ->.^ 44-44 .: ;* 

4.90 37.9*1 ii.*> 44-f* J'J-'J 8 ].* 

8.4^ 39.^7 M5.i6 44-< - w >'^* 'V-> M 

14.73 4<>.8fi Hj.3H 44. :w 

?i'S i5i; : : 

24^67 4i"<)3 33 ti 4 ; /. f i< - , , " ' KN 3 

^4-9* 40-99 311 /i I ^'^ ^'' l l < ;; t | >t ' 

26 '.93 9. '4 4.7*-* I>A - 0> * 

27,03 i5.i4 i^ r>l * WI 

27. 3Q 0.0 



SOLUBILITY OK POTASSIUM NITRATB IN AQUEOUS SOLUTIONS 
OF LEAD NITRATE AND VICE VERSA AT o. 

(Ehrtt. 



KAL1UM 



ftns. per 100 gaft. sat, sol. Solid 

' KNOT Pb(N0 3 ) ? ' Ptl * 



Qna. per 100 



sat. sol. 



Solid 
Phase 



o.o 



KNCL 



26.05 
36.27 



14.20 
8.95 



0.0 



37.37 

32-94 M 

29*63 " 

36.66 
14.86 37. 14 " * PblNO^ 

SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF STRONTIUM 
NITRATE AND VICE VERSA AT 20 AND AT 40. 

(Findlay, Morgan and Morris, 1914.) 



t*. 



i. per 10 
Sat. St 





KN0 3 . 


Sr(NOa) 3 . 


20 


22.90 


5-49 


20 


21.70 


9.17 


20 
20 


21,01 
I9.6O 


17.10 
31.24 


20 
20 
2O 


19.49 
I9-69 

17.56 


34.91 
39.56 
40.37 



Solid Phase. 



KNO, 



+Sr(N0 3 ) ? . 4 H 2 



t*. 

20 


Gms. ixrr roc Gms. 
Sat. Sol. 


KNO,. Sr(NOjt),. 
12.6$ 41.12 


20 
40 
40 


10 40.70 
30 . 26 23 , 70 
26.90 38.52 


40 


22.50 40.22 


40 


11.19 44-19 


40 


o 47-7 



Solid Phase. 



KNOa 



looo gms. HaO, simultaneously saturated with both salts, contain 552 gms. 
KN0 3 + 1074 gms. Sr(NOa)t at 25. (LeBkac and Noyes, x8^o.) NO 

SOLUBILITY OP MIXED CRYSTALS OF POTASSIUM NITRATE AND THAL- 
LIUM NITRATE IN WATER AT 25. 

(Fock.) 



Grams per Liter. 


Mg. 


Mols<u per Liter. 


Mol. per real 
TlNOa 


Sp. Or. 


MoJ. per cent 
TlNOt 


T"lNOa. 


KNOa'. 


liNO 3 . 


KNOj. 


in Solution. 


Solutions. 


in Solid Phue. 


o.oo 


351 


.0 


o 


.O 


3468 


.2 


O 


.00 


1.2632 





.00 


2-37 


3 2 9 


.0 


8 


9 


32SI 


5 


O 


43 


I.I903 


O 


.08 


6.IS 


332 


4 


23 


.1 


323s 


.1 


o 


.70 


I.I956 


O 


.20 


17.64 


333 


7 


66 


3 


3298 


.1 


X 


97 


I. 2050 





57 


49-74 


333 


3 


186 


9 


3294 


4 


s 


37 


1.2196 


I 


.78 


63.60 


321 


o 


239 


.0 


3172 


4 


7 


,01 


1.2436 


2 


,19 


86.18 


330 


5 


323 


.8 


3265 


.8 


9 


,02 


1.2617 


2 


77 


123.8 


428 


3 


465 


.2 


4232 


.6 


9 


.90 


I .2950 


J 

(27 


.00 

.04 


101.3 


245 


.1 


380 


.6 


2423 


3 


^3 


.58 


I . 2050 


93 


33 


116.1 


o 


.0 


4^3 


.1 


o 


.0 


100 


oo 


1 .0964 


100 


.00 



SOLUBILITY or POTASSIUM NITRATB in AQt/ioua SOLUTIONS 
OF URANYL NITRATS AND VrcB VKRSA AT 35 

(Colanl, I9fe.) 



Oms. per 100 
sat. solution 




Solid 



Otes. per 100 gni. 
3ft c. solution 



KNO, 



48.65 
53.88 
S3. 90 
54.21 
54.68 
56.08 



10.36 
10.40 

5*30 
3.36 
o.o 



KNO- 



K KALiUM 848 



NO 



SOLUBILITY OP POTASSIUM NITRATE IN AQIIVOUS SOLUTIONS 
or METHYL ALCOHOL AT 25. 

(AKrlof and TurcR. 193S.) 

in Aq. Solvent per ic0 *P Solvent 

0.00 3*774 

4.98 3*046 

9.45 2 '53 

21.04 1.532 

40.30 0.7130 

100 gas. Aq. 50 wt. % Ethyl Alcohol (C 2 H R OH) dissolve 3.7 gms. KN0 3 
at 20. (Wright, ' ' 



SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL SOLUTIONS 

(Gerardin Ann. chim. phy.U] St 5 '&S-) 
Grams KNOa per xoo Grams Aqueous Alcohol of Sp. Gr.: 



Wt ^* OHOH 


Oka. Hols. KNO 


in AQ. Solvent 


Pr 1000 tP. Solvent 


5994 

70.05 
78.46 
89.45 


0.3135 
0.1898 

o. 1123 

0,O607 



*' 


*. 0.9004 


0.0843 0.0793 o^>7a6 -ooS?* 0.^39 oJRo67 0.8429 
Wt 9 C Wt!'%. Wu%, Wt/%. Wu%. wT.%. \v".To. 


10 


17 


13 xo 7 4.5 3 x 0.2 


18 


22.5 


18.5 14.5 10 6.2 4.5 x.6 0.3 


20 


24 


20 16 ii 7.0 5 2 0.3 


25 


29 


24.5 20 13.5 9-0 6.5 2-S 0-4 


30 


36 


30 25 17 11.5 8 3.0 0.5 


40 


S 2 


43 36 27 16.5 n 4 0.6 




72 


61 50 38 23,0 x6 6 07 


60 


93 


79 69 52 31 .0 ax 8 I- 1 


SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL AT 18 






(Bodltnder Z. phyrfk. Ch. 7, 310, *yi.) 




SD. Gr. of 


Cms. par 100 50. S<iluti<n. sp. Or. >( Onw. pr r looker. Solution. 




Solution. 


CaHOH. HssO. KJScii". boWon. c^H^HT HjO. K.NO. 




1.1480 


89.80 25.0 X.OI20 23.33 69.81 8.06 




x.ioSs 


3.30 87.44 20. xx 0.9935 *8.xx 64.74 6.50 




I.IOIO 


5.24 86.26 18,60 0.9585 37.53 54.21 4.11 




1.0805 


8,69 83.18 x6.x8 0.9450 42.98 48.15 3.37 




* -0755 


9.06 83.10 15-39 0.9050 51.23 27.32 x -05 




1.0655 


14.08 77.93 14,54 0.8722 61.65 24.74 0.83 




I .0490 


16.27 76.36 12.27 0.8375 69.60 IJ-95 O-2O 




1-0375 


19,97 72.93 xo .8 




SOLUBILITY 


OF POTASSIUM NITRATE IN DILUTE KTHYL ALCOHOL AT 25. 






(Armitroiii aad Eyre, 1910-11.) 






Wt. % Gm, KNC), 






OJELOH in iHsr too (im. 
5fvent. St. Solution. 



o 27.77 

I.I4 26.69 



849 KALIUM K 

SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL AND IN AQUEOUS 

ACETONE. 

(Batnrick, 1896.) 

In Aqueous Alcohol. In Aqueous Acetone at 40*. 

Wt Per cent Cms. KNO, per 100 Gms. Aq. Alcohol Wt. Per cent ^*8* 

Alcohol. ' At 30 .. At 40. % Acetone. ^Solvent. " 

o 45-6 6 4.5 o 64.5 

8.25 32.3 47-1 8.J S*-3 

17 22.4 33.3 i6.S 38.9 

25.7 15.1 24-1 25.2 22.8 

35 11.4(34.4) 16.7 34.3 24.7 

44.9 7 xi. 6 (44 ) 44-1 17 

54-3 4-5 7-2(55) 53.9 11,9 

65 2.7 4.4 64.8 7.2 

75-6 1.3 2 (76.3) 76 3 

88 0.4 0.6(88.5) 87.6 0.7 

100 gms. H 2 saturated with sugar and KNOs dissolve 224.7 gnm sugar + 
41.9 gms. KNOs, or 100 gms. of the saturated solution contain 61.36 grrm. sugar 

+ 11.45 gms. KNOs at 31.25. (K^hler, 1897.) 

SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF METHYL 
ALCOHOL, ETHYL ALCOHOL AND MIXTURES OF THE Two AT 30. 

(Schreinemakers, 1908-09,) j^/% 

In Aq. CH 8 OH. In Aq. C 2 H fi OH. In Aq. (CHOH + C S H 6 OH ).* 

Gms. per 100 Gms. Sat. Sol. Gms. perjtpo^Gms. Bat. Sol. Gms. per loojGmi. Sat, Sol. 
CH,OH. " ^ 



' CjH 6 OH. 


KNOj. 


(CHjOH+QH^OH) 


KNOj. 


IO.I 


30.7 


o 


3 x -3 


23-8 


12. X 


12.7 


l8.Q 


32.2 


9 


29.2 


12. S 


43-1 


6.1 


41 


6.7 


56.9 


3-3 


47-8 


S- 1 


76.8 


0.88 


56.4 


3-S 


92.3 


0.15 


74.8 


1.2 



7-8 23.3 

17.3 16.3 

27.8 XX. 2 

38.4 7.7 

57 3-8 

98.58 0.43 

* The mixture contained 51.7% CH f OH and 48.3% C a H 6 OH. 

loo gms. trichlorethylcne dissolve o.oi gm. KNOat 15. (Wester and Btulni, 
loo cc. anhydrous hydrazine dissolve 14 gms. KNOi at room temp. 

(Welsh and Hitxlenon, 1915.) 

loo gms. aq. 40 weight % dHUQH, simultaneously saturated with the two 
salts, dissolve 13.74 gms. KMOs + 15-7^ gms. NaCl at 25. (Such, iSyft.) 



SOLUBILITY OF POTASSIUM NITRATI IK GLACIAL ACITIC ACID SOLUTIONS 
OF ANNOHXUN CHLORIDB AND or AMMONIUM NITRAT AT 35. 

t ana Hurablot, I'W.) 



Results for CH^COOK ^ N 4 Cl Results for CH,,OOOH * NH 4 M0 8 



Qua, por liur Soliu r liur 8ollo 



0.097 2.122 KNQ 3 0,00 

0.195 2.218 " 0.592 

O.e|05 2.464 " 2*035 

0.653 2.829 " 




K KALIUM 



850 



SOLUBILITY or POTASSIUM NXTKATX IH AQUEOUS SOLUTIONS 

OF IfKlTHAH AT 35. 
fPtUUCh I9flfl, IW.) 



fta. Mols. ptr 1000 0u> Hj.0 Solid 

KNOj 



3.772 
3.372 



0.0 

1. 1225 



ptr 1000 pit. H^O Solid 



1*911 

1*593 



KNO 



27 . 



RECIPROCAL SOUTH tm ar POTAISIUH NxTRAti AND UIXA 

Y TMI FXiK<IMO-Plr>INT MlTMOIi. 



KNO 



anna 



100 



. UNO,, pr Solid 

tOO pit. ttUuirt 



151.6 36.90 

1.36.1 32.64 

139-8 H09 

^Q I29.otr.pt. 



124.9 

120.1 



KMOj, isehi 
11 * 109.^5 T^tiec, 

H no,) 

115.6 

11 131*3 



27*79 



an - 



0.0 



tr. pt. is the point of transition of rhtwbohiiMl KNO S into rhombic 

KNvJ 

Fusion-point dau have t**n d^i^mintd for iht ffiU^lrti: fixtures: 

Hark. i9j s .f 
i 19*8.1 



Li NO, 
KOH S 



iCorvinti, 

(Ketorii lift ft Moles, 



NaNO 



, Liyfrtwm Mid MArt?i t iciu t 



(Ctrveui, Hi^ink) tooo; Ou*ruriiiU, j^ao; 

Briscti^ ami HAitflp, i^;i'i; GU**, L*ttourn and 
oAflgift, I9i|3 t J91"| I 

(L^y bourn *4 H4gin f 



4al Ridrticic, 
And CUrk, i*) 
(Roiitkotmki v 



19 ^^. 



OXIOE K f O 

The fusion-points of 



of it/) * V^O trt* gsv^n ly Cannrrl, 1928. 



851 KALIUM 

POTASSIUM HYDROXIDE KOH. 

SOLUBILITY IN WATER. 

(Pickering, 1893; at 15", Ferchland, 1902.) 



Gms. KOH per 
t o 100 Gms. 


Solid Phase. 


f. 


Gms. KOH per 
roo Gms. 


Solid Phase. 


Water. 


Solution 


Water. Solution. 


2. 


.2 


3 


7 


3-6 


Ice 


IS 


107 


51-7 


KOH.2H,rO 


2O. 


7 


22. 


,5 


18.4 





20 


112 


52.8 


* 


65. 


.2 


44 


5 


30.8 





30 


126 


55-76 


11 


-36. 


.2 


36. 


,2 


26.6 


KOH.4H 8 


32 


5 135 


57.44 


KOH.aH 2 Of 




7 


77-94 


43-8 


" 


50 


140 


58.33 


KOIUTiO 


33 




80 




44-4 


KOH. 4 H 8 0+KOH.2H S 


IOO 


178 


64.03 


K()H.H 8 O 


-23. 


,2 


85 




45-9 


KOH.aHjO 


125 


213 


68.06 


" 


O 




97 




49,2 


" 


143 


311, 


7 75-73 





10 




103 




50-7 


" 











Sp. Gr. of sat. solution at 15 * 1.5355. 

loo ems. sat. solution in H 2 O contain 50.48 gms. KOH at 15. 

(de Forcrand, 1909.) 
loo ems. sat. solution in H 2 O contain 53.1 gms. KOH at 15. 

(Greenish and Smith, 1901.) 
1000 gms. H p O dissolve 21.2 gm. raols. KOH at 35- 

(Axurluf ana Sliart, 1937.) 

SOLUBILITY OF POTASSIUM HYDROXIOB IN 

(Horn, to:*?.) 



Q Hhs. KOH Pr 


Solid 


ft**. KOH per 


SoHU 


1 100 i 


jms. aac. sol. 


Phase 


IOC * a - owe,, y 


ol. Ptw 





^18.85 K< 


DH.aHgO 40 


$8.01 


KOHjy) 


11.5 


5i07 


65.3 


60.36 


" 


25 


54.23 


80 


6l .73 


" 


33 


57-53 


" KOH. HO 100 


6S-15 


11 



The original results are given in terms of K f O 

FREEZING-POINTS OF AQUEOUS SOLUTIONS OF POTASSIUM HYDIIOXIDE. 
(Klein and Bvanborg, 1020.) 

t* - O.:H:J. ~n.ft7.>. \.m, 

Gms. KOH per 100 cc. sol <>.56u i.4<>'J '^.8o"> 

SOLUBILITT AND TRANSITION-POINTS or POTASSIUM HYDROXOI IN WATUR. 

(:a ilb at a. Odtt and FurulUiWft, 10>,?.) 
t o Oma. KOH per 100 pi. ftt. ol. Solid >'hao 

25 S3-1 KOH. all 

27.27 tr. pt. KDH.aH.O * KOH, i*HJ) 

33.113 M KOH.iiHgO * KOH.H.O 

37.33 . (unstable) KOH.aK^O * KDH.H^O 

Data for the system KOff * NH^ * H^O are given by J&necke, 1933 (&l* v 
Weighed amounts of the three components were placed in small glass 
ampules which were then sealed. By warming or cooling the** ampules, 
the upper and lower temperatures were determined at which a wild phase, 
two liquid layers or a combination of solid and liquid layers appeared 
or disappeared. The temperatures at which certain of the d^npules ex- 
ploded are also given. 



K KALIUM 

SOLUBILITY OF POTASSIUM HYDROXIOK IN AQI?KCK?S SOLUTIONS OP ETHYL 

ALCOHOL AT yf* ttfciuai, **JR,J 

to*Pj[^L^ ^ m Ph- tim!< *' lw c ' nw " Sttl ^ 



55.75 O 44-atS KOH.IV> -7-<>7 <*MM Jr. 41 KOH.a!LO 

54,81 0,43 44.?6 " 4 7 - 73 01 negative* 

Two liquid Uyera are formed here, j(i J}J Hi t>$ M 

31 57.50 1X-50 KOH.iHit) 

28.99 6 S-7 S-<>4 

* Ndttttivetmau-ountolrractmn KOH-H'|HtO!! ~*t',Ht)K Hlif,) 

SOLUBILITY or PoiASsnm fffwtwiM f MIT?L ALCOHOL AM IN KTHYL ALCOHOL 



The mixtures w*r* ;tltkn occAHtcmAlly ilyriw^ Atnmi iltret* 

a. or >*, KOH p*r tooi 

-- 



28 Methyl Alcohol CH^OH uin \ .^.^ ?ag 

28 Ethyl Alcohol *>*U^ * o< * ar ^* J ? r i 5,37 



POTA8XH HYDHOXlOt X A^K^US .SOLUTIOMA <>r ACITOHI AT 0*. 



The binoddl curve I*AS ilei^wiw^tl hy ittrfttiog Aertiine into aqueous KOH 
solutions until 4 perwMt^m separation latu iww l^^rn occurred. Tie 

lines r *,were located by e*i f wiiiwrft which ytrhl^^ 
of the two layers to be u*Hi for inr*%tii| thi* Kdl in t?iw:U. 

OM. ptp 100 flte*. tr 100 ^1*, Hr too te' 



o^ 80*1 a*a m-t i*. i si i r ti.o * * 

0.6 70 S 3*0 W4 1**-^ *I*S J7j 2,0 

0*7 70*S ^*i 41*7 17*9 7.H 48.4 1^ 

U7 5S*^ 4*8 41*1 J**7 ^.% jH.H 

2.0 537 S,a J6.6 JU| i.j i7*l * 

Data for equilibrium in ft* y*trm jmt i?***ittitt hv<tfoiir ( iihrmi), water at 25* 
are given by van Mtur* (i^ifii, 

Freexing-point clalii ftir KOH + MH! Kflil I N.iOH it'r given by 

von Hevesy (1900). Krtiulu fur KOH -f Kf iifr gtvnt l*y %-4f|**t (1915). 

POTASSttJtt DihydroiM riH-Pi4fl KH^rt 1 ) 

SOLtfUXLITY 01^ P(tfAIl|iX iMftyoirkfcft* PHitimArit IH 



M^P, B| rv 4 p, -. ^ ^ .. ...^ 

100 iM. M&, Mi. | P, MU Ml. * 100 |P. Mi, 

o ia88 (ta48t 3^ ao*04 tatuori m ji.ni 

5 l^00 "JO lltQ'O 60 '|' : li|ii 

15.SO IS 70 J7.0S 

15 l6.87d6.78) 40 |<!0 to Hi. |0 



The rtsttlu U pirtiifetsi* art fey MA ftM*t*r ifj*i^ TIi earlier 

results of Ntti)Mi wit WH; Jtetclr, 
ftskenwy and Ifttsltr, if 30 rt tot it nli 

especially &t tbt ioMrr iMptr*tri 



853 KALIUM K 

SOLUBILITY OF MONO POTASSIUM PHOSPHATE IN WATER. (Apfol, ion.) 

Mols Rift 1*0 1 Cms. KU,POt Mols. KH, PO V ttms. KH, P0 4 

Vr 1000 Jms. per 100 gms. Pr 1000 urns. per 100 tm*. 

. sn t. sol. sat. sol. t"- - SJ l - * l - sat - *" 

0.77 10.48 5o a. ^9-^7 

7 .. 1.465 19-9^ 7 v>..693 36. 67 

2 5^ 1.48 -20.15 83 3.oB 4i.94 

SOLUBILITY OF MONO POTASSIUM PHOSPHATE IN AQUEOUS SOLUTIONS OF SALTS 

AT 25. (Apfd, 1911.) 
GIWH. salt Gms. KH 3 P0 4 
per 100 urns, por 100 KIUS. 
Salt. s?i. sol. snl. so). 

None .... o.o so. i:> 

K 2 SO.v... 1.39 i9.4f> 

... 3.i3 iB.9,4 

... 6.27 i 7 . 70 

... 6.79 17.02 

... 6.27 16.74 

In the case of the solubility in aq. K a GQ$ carbon dioxide is liberated and the 
results do not show equilibrium. 
SOLUBILITY OF POTASSIUM ACID PHOSPHATE, KHaPO^HjPO^ IN WATER. 

(Parravano and Midi, 1908.) 
Determinations by Synthetic (sealed tube) Method. 

Gms. J-?? 11 ?!. 

Solid Phase. t*. 



Salt. 

KNO-j 


(Jms. suit 
per 100 gins, 
sat. 1. 

5.56 


<;m, KH > I0 4 
per too gms*. 
nat. sol. 

16.33 








CH 3 COOK. 
K s Col....l 


4.91 
i .66 ( n.ajT* 


1 7 4 3 
1 4 4 ' * 
28.01 
3r.8"> 



Sat. Sol. Sat. Sol. pn 

'-0.6 3-337 Ice 65.2 68.44 

-2.5 12.13 " 78 72.43 

-6.7 29.43 " 87.5 77.6 

9.2 36.98 " io's.5 8s-Q 

-13 Eutec. 44 " +KH 8 P0 4 120 tr. pt. 92. i 

o(?) 45.8 KH,P0 4 135 Q6.X 

+ IO.Q 50.3 " 139 IOO 

EQUILIBRtHM IN THE SYSTEM POTASSIUM OXIDE, PHOSPHORUS 
AND WATBR AT 

19P7.) 



The results are presented in terms of Gms. of H^O required to dissolve 
ioo gms. of mixtures of KJD + P^O C containing determiner! percentages of 

y>. * 

Percent K ? 3ns. H^O required to aistsolvo Percent K_0 Oma. t\J) rt^ulrtd co ditto Ivt 

in dissolved too gwa. K^ *Jjp^ &L: ln AliMlvtd top * 

-----^ """"" ..... ...... * - ...... ~ 



2. a 73S 'I78 58. S B2.0 Ba.O 

10. 44 44 O 6l.O lOif.O 80 . 2 

13-1 13l0 92.0 63.0 147*0 101.5 

19.5 80 58.0 66.5 1S3.0 U7. 5, 

24.7 172.0 121.0 68.5 in-0 119.0 
25*0 63.0 59. 70.8 l6o.O 118.0 
30.0 360.0 l8$.0 73. S 151-0 Ut).Q 
33*0 280.0 249-0 76.1 153.0 1*9.0 

39.8 460.0 43S.O 79- S 171.0 lll.Q 
48.3 363.0 292.0 82.2 173.0 110,0 



KALIUM 



854 



The diagram drawn from the above results showed the existancc in the 
strongly alkaline solutions of the hitherto unknown K^PO^.SH^O. This 
salt was obtained in pure form ami its solubility in water determined 
with the following results. 



100 



Mt * solution 



n O.o 
57.0 
50,7 



SOLUBILITY OF POTASSIUM Ann Pnosrii ui- , KlhVi 

PHOSPHORIC Ani. 

(Pamvano ami Mvlt, iyoH ) 
Determinations by Synthetic tube) Method, 

tnw, p too (Jnw. Sal Solution, 



l'Oi, IN ANHYDEOUS 



*", 


kH v pcviiiK) 


$cfi s ro 4 , 


38.5 


18,17 


10,5.0 


84 


58.42 


33 c )7 


no 


77 "S3 


4S-oK 


126,5 


92 , 26 


S-9 



EQUILIBRIUM IN THE POTASSIUM UYDKOXWK, Pftmriiawc ACID, 

WATKK AT 25**. 

(IVAnnawl Schifiner, 1910*; Pa Aw. 1*114 I 

The results of these tnventtgiiton fuiti#fafirtly when plot ml on crow- 

section paper. The following figure* wttrt rrail frmi t tht* rtirvrs, Some uncer- 
tainty exists in regard to the aohd in ctmtat'i with twine* of the Holutiona. 

Moll. per i<xx> Gmi.^t.Sd. - - . MU- nrr t*mt . Si S*t. 



K. 


K). 


9.6a 


O 


9.76 


0.24 


9- x S 


o-S 


8.2 


X 


7-5 


x*S 


8,2 


2 


7-5 


25 


8.8 


2,9 


9-7 


2.9 


9-5 


3 


8.5 


34 


8 


3-6 


7-5 


3-7S 



4-K,WV,$HiO 



k, 


Hi, 


7 


4 


6 


j.6 


S 


:t *s 


4 


2 65 


3 


2 


2 


1.7 


i-S 


x-S 


1,0 


J 


2, t 


4 


2 S 


6 


3 


8 


I , (15 


Ci 


i '35 


H 






or RIUK>(?) 

M (?) 

(?) 



fCPtrker) 



Futon-point datm for KIK>t + K*P|C>t are given liy I\trr,4vniwi ami Calcagni 
(1908, 1910), 



855 KALIUM K 

EQUILIBRIUM IN THE SYSTEM POTASSIUM DIHYDROGKN PHOSPHATE 
AMMONIUM DIHYDROGKN PHOSPHATR AND WATER AT o. 

(Astcenasy and Messier. IDTSO.) 

This pair of salts form a continuous series of mix-crystals. The 
results are expressed in accordance with the terms adopted by Janecke. 
Additional results for the quarternary system (K, NM 4 ) (CljH^PO^ ) * H^O 
are also given. 

a. of Mols. KH ? P0 4 per Mola. H ? co dissolve Mol. Perctnc KH p P<> 4 

sat. 100 mols. of dissolved 100 mols. of In ai Mix-Crystals fora- 

SOI. KH p P0 4 + NH N PO, "W * *W< lftg aiS S0lid PhMt 

\ 1 c *\ 

1. 1043 0.0 2815 0.0 

1.1312 12.4 2<(5Q 6.5 

1.1350 15.3 2350 9*0 

i.ifin? iB-2 2280 13.2 

1.1S68 26.4 2200 23-2 

1.1574 31^2 2130 30.7 

I.l6ll 35.2 2105 35.9 

1. l604 36.4 2120 0,2,4 

1.1603 38.1 2130 a8.8 

1.1571 44.2 2240 71.1 

1.1577 '49.3 2325 8l.9 

1.1472 $4^7 2540 87.8 PC) 

1.1393 67-4 29SO 94-5 

1.1169 80.6 3400 96.7 

1.1151 100.0 4125 100.0 

Additional data for the solubility of mixtures of various Potassium and 
Ammonium Phosphates in Water at o and 2$ are given by Janecke 1927. 
Attention was directed particularly to the system K PC) MH H PO * I! 
in which the following solid phases occur at either o or ay ; K fr) .8ft 0, 
K^RP0 4 , (NH 4 ),P0 4 . 3 H 0, <NH 4 ) p HP0 4> KH p P0 4 and NH H p Pt) 4 . The itc?ermi na- 
tions were made by the synthetic method. The solid phases wer< identified 
by the polarization microscope. Nine binary mixtures composed of the 
three potassium and three ammonium salts were studied. The results how- 
ever are given in an abridged form chosen to show the most important 
features of the system. 

SOLUBILITY OF POTASSIUM DIHYDROGBN PHOSPHATE IN AQUEOUS 
SOLUTIONS OF HYDROGEN PEROXIDE AT o. 

(Menzti & 



Owia. per 100 gn. sac. sol. 



0.0 \2.t\B 

6.S90 l607 

8.242 18.67 

SOLUBILITY OF POTASSIUM DTHYDRODKN PHOSPHATE IK 
AQUBOUS SOLUTIONS op IJRKTHAN AT 25. 
(p*iuzci, im, 1939) 

Om. Hol. pr 1000 ws. H Solid 

^^^ ^^ 

1.82 o.o K* 1 * 1 * * 

! 29 1 122$ " 

75 5^0l " 

0.139 22.25 rf 



KALIUM 856 

POTASSIUM HYPOPHOSPHATE, etc. 

SOLUBILITY IN WATER. 

(Salzer Liebig's Ann. 211, i, 8a.) 



Pota 


4 

POTA 


Salt. 


Formula. 


Cms. Salt per 
Cms. HbO. 


too 


Cold. 

ssium Hypophosphate K 4 P 2 O fl .8H 2 O 400 
Hydrogen Hypophosphate K 3 HP 2 Ofl.3H 2 O 200 
Di Hydrogen Hypophosphate K 2 H 2 P 2 O .3H 2 O 33 
Tri Hydrogen Hypophosphate KH 3 P 2 O 6 66.6 
Penta Hydrogen Hypophosphate K,JH[ g (P 3 O 8 ) a .2H a O 40 
Hydrogen Phosphite KH 2 PO 3 172 (20) 
* Hypophosphite KH 2 PO 3 200 (25) 
' Hypophosphite KH 2 PO a * 14.3(25) 

* Solvent alcohol. 
.SSIUM PerRHEMATE KReO . 


Hot. 

100 
200 

333 

28 



SOLUBILITY OF POTASSIUM PBRRHRNATE IN WATRR. 

(HBleaann and Kleese, 1950.) 

Tlie previous determinations, at temperatures up to io<f by Puschin 
and Kovac, 1931; lewtno , Noddack and Noddack, 1931; and Roth and Becker, 
19321 although varying among themselves, give, when plotted, average 
values which agree closely with the present very careful determinations. 
The determinations above 100 were made by the synthetic method. The 
solid phase is KReO^ in all cases. 



d. of sat. 


fas. KR*0. Pr 


te. 


KP0 4 per 


*, 


OB. KRt0 4 ptr 


C solution 


100 gns. sat. sol. 


100 8 


3. sat. aol 


L 


100 <0aa- Mt. sol. 


-0.06 (Eutec) 


0.34 


109 


12.6 


366 


84.6 


*io.s 1.0028 


0.62 


112 


14.0 


401 


89.3 


25.0 1.0067 


1.19 


154 


26.3 


445 


94.4 


50 1.0128 


3-19 


194 


36.7 


'l $6 


95 4 


60 1.0210 




220 


50-7 


470 


96.8 


75 1.0303 


6.95 


239 


599 


498 


97-4 


85 1.0412 


8.98 


290 


71.9 


58 m. 


Pt. 100. 


99 1.060 


12.20 


335 


80.1 






i liter 89.7 Wt 


. percent Ethyl 


Alcohol, 


C ? H 5 OH, 


dissolve 


0.302 gm. 


KRe0 4 at 18.5. 


(Tollert, 1932.! 











POTASSIUM SULFTOE 



Fusion-point data are given for the following systems: 
K g S + K g S0 4 (Garibeau, Kolb and Kroll, 1938.) 
K p S S (Thomas and Rule, 1917; Pearson and Robinson, 1931.) 



POTASSIUM Antimony SULFIDE 

POTASSIUM SulfoANTmONATE K s SbS4.5H a O. 

SOLUBILITY IN WATER. (Donk, 1908.) 



'2 I '% 9 '5 Ice 34 62 

2 -^ I 7-I " 10 65.5 Ka$b$4.6H a O 

2 4 24 ' 2 " - 4-5 69.1 

7- 2 35-4 " o 75.4 

-10.6 42,9 + I0 7 6. 2 

""I3-S 4^.8 ^o 75.1 

""2J 52.6 U 50 77-7 

-28.8 59.6 80 79.2 



857 



KALIUM K 



SOLUBILITY OF POTASSIUM SULFOANTIMONATE IN AQ. SOLUTIONS OF 
POTASSIUM HYDROXIDE AT 30 AND VICE VERSA. 

(Donk, 1908-) 
Q^^^&S^J^ s^p^. GmS g per,ooGms.S^Sol. ^ phw . 



K,SbS 4 . 

75 

68.4 

56.8 

So-9 
37-7 



KOH. 
O 

3*4 
ii 

16.1 
25-S 



KaSbS 4 



KjSbS,. 


KOH. 




19.8 


40.5 


KsSbS* 


ii. S 


49-9 


" + KOH.aHO 


9.4 


49-? 


ICOH.aWsO 





56.3 


44 



SOLUBILITY OF POTASSIUM SULFOANTIMONATE IN AQ. ETHYL ALCOHOL. 

(Donk, 1908.) 

Results at 30. 

Gms. per 100 Gms;. Sat, Sol 

Solid Phase. * v CK ^ * 

K. a bbb 4 . 

O 



K,SbS 4 .sH,0 



Results at 10. 
Gms. per 100 Gms. Sat. Sol. 
'K,SbS 4 . C 2 H 6 OH. 

o 94 

o 90.5 

Two Liquid Layers Formed Here. 

69.2 0.8 

76.1 o 

Composition of the Liquid Layers. 
Gms. per 100 Gms. 



97 



phlffle 
KiSb$i.jHW> 



Two Liquid Layers Formed Here. 

75.1 o 

Composition of the Liquid Layers. 
Gms. per 100 Gms. 



^ Alcoholic Layer. 


Aqueous Layer. 


Alcoholic Layer. 


Aqueous Layer, 


K 3 SbS 4 . 

2.2 
4.2 
27.4 


CjHsOH. 

85 
54-7 
46.9 
16 


67.4 

49 
45-6 


CjHjOH. 
1 .1 

3-4 

3.8 



O 
2.2 

8.5 


C,H 8 OH. 
93-1 

56^8 
41. 1 


KiSbS. 

70.5 

65.2 


t:,HOK. 

0.5 
I .2 

5-7 
9.2 



12.7 31.1 

SOLUBILITY OF POTASSIUM SULFOANTIMONATE IN AQ. METHYL ALCOHOL AT 1 

(Donk, 1908.) 

Composition of the Liquid Layers. 
Grm. per 100 Gm. 



Cms. per 100 Gms. Sat. Sol. Solid Phase. 


Alcoholic Layer. Aquwu 


r ,,. . ,-, .^^ 


' K 8 SbS 4 . 


CHiOH. 


XSbS,. 


CHjOH. 


Ki^bSi. 


clwii^ 


o-S 


99.5 K,SbS 4 


5 


82.5 


62.5 


8 




99-5 


4-ft 


76-3 


* * 





i-S 


93-9 


7 


66.9 


. . * 


* , . 


1.8 


92 


13.6 


54 




. . . 


Two Liquid Layers Formed Here. 


19.1 


45-5 


. . . 


* . 


62.7 


7 . 5 K,SbS 4 .9H/) 






31.1 


3* -3 


68.4 


3-5 




. . . 


41.1 


22. a 


75-5 


o " 






47,2 


18.2 


Two Liquid Layers Formed Here. . . . . 


57-* 


ii, i 


0-5 


98.1 











KAL1UM 

POTASSIUM SULFITE K 2 SO 3 . 

SOLUBILITY OF POTASSIUM SULFITE IN WATER. 

(Fcerster, Brosche and Norberg-Schultz, 1924.) 

The determinations were made with the greatest care. Constant stirring was 
employed to secure saturation and an atmosphere of hydrogen to prevent oxidation. 

Cms. K,SO, per Solid 
100 f?ms. sat. ol. Phase. 

5i.o K,S0 3 



i.6o 


Cms. K,S0 3 per 
100 gius. sat. sol. 

5.78 


Solid 
Phase. 

Ice 


i ll 


. . . Q . 2O 




../i. 

.{ 10 


... . i3.37 


w 


5 7 i 







6 8i 


'2O . 02 





10 88 


26 . 70 





1 4 06 


3o.6 





3r o 


. .. 44.0 


t) 


45.5 


Euiec. 5i.o 


H-K, 



-16 . . 


... 5 1 . 3 






3 o.. 


'> i . 3 > 


-H" O \ . . 






> f 3? 


3o.o. . 


5 1 .76 


5{./{. 


. ... 5 1 . 90 


97. -A.. 


52.88 



EQUILIBIIUM IN THE SYSTEM POTASSIUM SULFITB, POTASSIUM OXIDE AND WATER. 

(NtilBl. 1937.) 



per 100 gs. sst. sol. 



ORB. par 100 gms. sat. ool. 



' K_0 K_SO_ Phas* 





0. 





47. 


52 


K.SO, 


" 


40. 


71 


0. 


43 




KOH. 


2H p O 


M 


41* 


01 


0. 





KOH. 


an 


* 




11.5 


0. 





48. 


06 


K^SO 


i 






" 


42. 


m 


0. 


48 


'N 




OH. 


sHpO 


11 


42. 


87 


0. 


p 


KOH. 


2 H 


o 




25 


0. 





49- 


01 


K^SC 


1 






it 


45* 


03 


0. 


47 


M 


+ 


KOH 


.2H g O 


n 


45 


51 


0. 





KOFI. 


2H 


.0 




33 


0. 





49. 


99 


K*SC 


1 








47. 


81 


0. 


37 


' 


+ 


KOH 


.HO 


" 


48. 


16 


0. 





KOH. 


, 


+ 


KOflail 


" 


48. 


29 


0. 





11 




* 


KOH. 2! 





V 


K^Soy 


40 


0.0 


SO. 37 


" 


/I8.32 


0.40 


H 


48.71 


0.0 


65. 


3 0.0 


53.27 


M 


50.14 


0.45 


" 


50.65 


0.0 


80 


0.0 


53-15 


H 


51-50 


0.39 


11 


51.8l 


0.0 


100 


0.0 


55.53 


rt 


54.29 


0.40 


M 


54.67 


0.0 



Solid 
Phase 



+KOH.H.O 

KOH.H.O 
K f S0 8 f 

11 ? KOH.H 
KOH.H .0 



KOH.H 



KOH.H 



KOH.ILO 



KOH.H n 



EQUILIBRIUM IN THE SYSTEM POTASSIUM SULPITB, SULFTIROUS ACID AND WATER. 

(Hftlsl, 1937.) 



QMS. per 100 gma. sat. sol. 



i r~ 


HSO_ 


K 80 ' 




? 3 














0.44 


50.36 K^ 


" 


7.49 


14.06 K 2 


11.5 


1.11 


50.96 K g 


25 


1.83 


51.92 



Solid 
Phss 



Qns. par 100 p\s. sat. sol. 



Solid 
Phase 



40 2.64 

6S.3 4.37 

80 s48 

1 00 7.0 



S3*01 

55-12 
55-82 
56.60 



SOLUBILITY OF POTASSIUM SULFITE IN AQUEOUS SOLUTIONS 
OF TERTIARY BUTYL ALCOHOL AT 30. 

(cunnings ana Bobbins, 1930.) 



Wt. Percent 

(CH^^COH 

in Aq. Solvent 

0.0 
0.4 
0.9 



is. KgSO^ Pr 
100 tP*. 
aau aol. 

51.76 

34.2 

26.7 



Wt. Percent 
(CH S ) 3 COM 
in Aq. Sol vent 

9.1 
16.1 
18.9 



is. K 9 SO^ pr 

r 3 

100 

flftC. SOl. 

9.8 
5-8 

4*8 



859 



KALIUM 



POTASSIUM I>yro SULFITE KS S S O S ami K.S.O^IUo. 

boi.uun.iTv m WATKR. 

(KoaHter, Broirho.,,,, Nwl>< , S( . h||1| im 

The numerous determinations of tW .,i i \ j i * n 

values ad from the curves. ""' ftulhoni wt ' r<! P lo " wl " (1 lh Iow.n,j 

Results for K,S 3 O. i>.....i., f .... i. o ,-v .,, ,, ^ 



, ,., ,, . nesuiis JOT ivo . i.^, -/a iisv./. 
Gms. K a S 9 0. per Solid , . ., o /j *v 
t 100 gms. sal. sol. Phase. <tus. K^S^i., ptn- Solid 
.)>! * - HM'Kinx. sni. sol, Phnso. 
- 1-07 J-7-i lce - i x i.. 




6.8 > '" *^ s 


- 4.o 


., t> "*">*., o ~* ,*> t, 
i-^.B _ / o r. . 


J . 


i7. r > > - 


5.6 Kutee. 
3<> 


i/ c /'*"" 2 ' " ^'OKuttic. 18.0 ! K'S*O- , a .' 

20.7 K,b,u, . . 4>0 K.s.d..vii.o 


: o.o 


'^'1 . ( II rj ' - " 1* 
tt ' ** - * ' " ' ' " *.)*) M 


10. 


2f). r > -j., * < o > ^'J 


'>O 


3o. 8 > , * ' ' 


j.5.o 
3o.o 


3.i- J-;; M- ;; 


,{o.o 


'M)*^ " M ^ % 


5o.o 




Go.o 
80.0 


46.0 ,. ;:.'" 7-' 
si. ) .,-" ^;- 


94-0 


15. ) .. '" "' 



100 RNS. liquid Sulfur Dioxide 



with Po t as .stum F*y ro S 

POTASSIUM Sodium SULFITK KN;uH^A \ tin 
100 gms. Ii 2 dissolve 69 gms. of the * iV^tf"* ' 



at 



(Schwickcr, 



POTASSIUM SULFATE 

SoLUBi UTY IN w . 

(Mulder; Andmc, 1884; Trevor, x8gx Tildciiand Shrnn oi . i r 4 , 

'^wnstonc, 1884; Berkeley, 11104; iwr ;ilii J-.tanl, iXi ) 



t. 




urms. 


JS^U 4 


pericx 


3 urns. 


C 
40 


^ms, K,SO 4 : 

'""'w^r^ 

14-76 


[*r f oo C"mw. 

^^^wnkMin^nwnwMn, 

S<Uiti<m, 

12.86 


t e , ^. 
cp 


Jmi. K-jSO, 


IMT nvUiir 


' Water. 

7-35 


Solution. 
6.85 


Wul-r, 

22. 8 


Solution 

18,57 


10 


9 


.22 


8 


44 


5 


16, 


50 


14. 1 6 


too 






20 

25 
30 

r ^ 


ii 

12 
12 

r . 


.11 

.04 

97 

. t __!.. 


1C 
10 

ii 


75 
.48 


60 
70 
80 

_ j. . ^i _ *. 


18 
19 

21 


.17 

75 
.4 


*5*3 

16,49 

17,63 


1 20 
143 
.170 


2H.H 


20 . t)4 
*?4 7(1 



The determinations of Berkeley ( i Q O .N 
are as follows: 

Sp. Gr. of Sat. Cms. K t SO 



1.083, 



. . . , 

were mutta with exrt*put)tULl 





Solution. 


100 Gms. HO, 


t*. 


Kp, (k, of Sftt. 


(iwa. Iv-jHC^ }rr 


0.40 

15-70 


1.0589 
1.0770 


7.47 
10-37 


S.() S 


Slutitm. 


tK.oi 1 


31-45 


1.0921 


^3-34 


o() , ^O 


I , 1 157 


. . , So 


42.75 


I . 1010 


iS-Si 


xo i , T b 'P 


>t. 1, . I 2O7 





Individual determination in gotxl 
Blanc and Schmandt (^"JjOr 
(1910); Smith and Ball (1917). 



t 

th . c ; l , lw I w v an ' Kvi-n by Li- 
09OI); ()ilw (iyM"HJ; Nat-krn 



KALJUM 860 

SOLUBILITY op POTASSIUM SULPATE IN WATBR. 

The closely agreeing determinations of Caven and Johnston, 1927, 1928; 
Wright, 1927; Flttttmann, 1928; Blasdale, 1923; Hill and Moskowitz, 1929; 
Starrs and Storck, 1930; Malhorta and Suri, 1930; Ben rath and Wazelle, 
1939; Babajewa, 1913; Rakowski and Babajewa, 1931; Schr6der and Schlack- 
mann, 1934; and Benrath, Gjedebo, Schiffers and Wunderlich, 1937 for 
temperatures above 100, were plotted and the following values taken from 
the average curve. 



c 


Qns. K ? S0 4 per 
100 8Ps. sac. sol* 




10 


6.9 

8.5 


15 


9.2 


20 


10.0 


25 


10.75 


30 


11.5 



40 
50 
60 
70 
80 
90 



100 tfa. sac. sol. 

12.9 

14.2 

15*4 

16.55 

17.6 

18.6 



100 
179 
208 
245 

292 



100 wa. sac. sol. 

19.4 
25-4 
25.7 
25-9 
26.0 



310 
327 
337 

357 



QMS. K ? S0 4 per 
100 ws. sac. sol. 

23.3 
16.2 
12-3 

8.36 

3*9 



The densities of the saturated solutions are: 
at 20 and 1.0853 at 25. (FlOttmann, 1928.) 



1 .0757 <*t 15, 1.0807 



Data for the Solubility of Potassium Sulfate in Wa\er -at 25 and under 
50 Pressures up to 10,000 bars (metric atmospheres) are given by Adams, 1932, 

EQUILIBRIUM IN THE SYSTEM POTASSIUM SULPATB SULPURIC ACID AND WATBR. 

(Babajewa, 1931.) 



Results at 30 Results at 50 Results at 75 



QMS. per 
sac. A 


100 gns. 
sol. 


Qns. per 
sac. 


100 fps. 
sol. 


Qtas. pr 


100 dJna. 
sol. 


r H 2 80 4 


w 


' V4 


W 


' H 2 S0 4 


vV 


0.0 


11.50 


0.0 


14.16 


0.0 


17. 10 


5.38 


15.70 


4.92 


18.66 


6.77 


24.27 


8.75 


18.80 


7.45 


20.09 


8.07 


25.55 


11.22 


20.80 


11.60 


26.03 


8.96 


26.38 








14.40 


29.6l 


12.43 


31.24 


12,00 


22.00 


16.40 


32.80 


18.03 


40.43 


17.6l 


22.56 


19.37 


33.80 


18.80 


40.81 


20.95 


22.99 


21.49 


35-37 


21.03 


42.76 


21.20 


24.80 


22.40 


36.40 








23.49 


17.64 


23.21 


31.66 




















24.40 


46.38 


28.41 


10.83 


23-73 


30.47 


25.16 


42.82 


33.92 


6.43 


24*42 


28.15 


26.97 


37.27 


37.38 


3.56 


27.63 


22.03 


30.05 


28.80 


52.20 


2.18 


32.49 


14.25 


40.00 


13.98 


54-59 


2.00 


36.80 


9-27 


54.23 


8.88 


63.16 


3-35 


43.79 


6.34 


60.48 


9.50 


68.93 


4.84 




















56.13 


4.41 














63.98 


5-75 














68.08 


9.96 








75.67 


4*12 


72.00 


19.78 








. 


- 


74-52 


13*41 


- 






Solid Phase 

ac each 
temp era cure 



T K0O*j .Qj\nou 4 

K.S0..6KHSO. KHSO 



K*so*".Kiisb/ 

4 KHSO 4 



Kx 
KHSO. 



KHSQ. 



K x is perhaps the hydrate K g S0 4 .KHS0 4 .HgO. 



* 861 4 KALIUM 

SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC 

ACID AT 1 8. 

(Stortenbecker, 1902.) 



Mols. per 100 Mols. 
K,S0 4 +H 2 SQ 4 +H 2 0. 

K 2 SO 4 . H^SOT- 

1. 10 O 

1.59 0.95 

2 . 49 2 . 70 

2.75 3.17 

2-75 3-74 

2.83 5.08 



SoUd Phase. 

K 2 S0 4 



K 2 S0 4 .KH$0 4 



Mols. per 100 Mols. 



JK. 2 JSO 4 , 


H,S0 4 . 




2,80 


5-79 


K a $Q 4 ,3KHS0 4 


2.6l 


5.61 


KtSO 4 .6KHS0 4 


2.25 


6. 19 


f.|CHSO 


1. 08 


7-94 


KHS0 4 


0.77 


9-2 


it 


0.44 


22.7 






SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF SULFUEIC 

ACID AT o. 

(D'Ans, 



Mols. per 1000 Gms. 
Sat.jSol. 

K a S0 4 . H 2 S0 4 . 

0-53 0-37 

0.64 0.75 

0.74 I. 08 

0.73 I.I3 

0.71 1.44 

0.69 1.66 

0.69 1.88 



Solid Phase. 
KS0 4 



Mols. per xooo Qms. 
Sat. Sol. 

H,SO. 
2. 12 
2.29 
2.30 
2,48 
3-04 
4-43 
$.27 



0.61 
o.54 

0.43 
0.28 
o.o 
0.09 



Solid Phase. 



1 +KHS04 

KHSO 4 



K a and Kb are acid sulfates between KiH(S0 4 ) 2 and KHSO*. Their 
tions were not determined. 



SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF Sui PURIC 

ACID AT 25*. 

(D'Ans, igoga, 1913; see also Hers, 191 1-12.) 



Mols. per 1000 Gms. 
Sat. Sol 


K 2 $0 4 . 
1.27 


H,bO, - 


1-33 


1.99 


1.24 


2,03 


I.I3 


2.17 


1.04 


2-35 


1.032 
0.67 


2-345 
2.83 


0.22 
0.15 


4.13 
5.36 


K,S0 4 . 
O.I7I 


H,S0 4 +SO,. 


O.IOO 

0.266 
0.182 


6.*6o 
6.91 
7.26 



o. 167 

0.201 



7.62 

7.88 
8 



Solid Phase. 



K 8 S0 4 +KH(S0 4 ), 



Ky 



4-KHSO, 



KHS0 4 



4-KH 8 (S04) s .%0 



Moli. ptr 1000 Gnu. 



0.250 


Vxo* 


0.352 


8.15 


0.364 


8.16 


0.341 


8.2Q 


0.322 


B.33 


0.325 


8,45 


0.346 


6.62 


0.384 


-S7 


0,412 


8,71 


0.5% 


8,82 


0.880 


8,65 


0.899 


8.63 


0.882 


8.70 


0.561 


8.06 


0-365 


0.8o 


0.43 


9. 78 


0.665 


9- Ho 


O.Q37 


9.66 



Solid 



" +KH|(SO)9 



<( 4-XHSOr 



was not determined. 



K 8 H(S0 4 )s and KHSO 4 of which the exact com- 



K KALfUM - 

POTASSIUM Bi SUtFATB K"!IS0 4 

SOLUBILITY OF !\>TA8.SXHM HXHC'tKATR IK tf 



OBIS. KH 4 ptr >. 4 ' *ts. KHSO ptr 

1 100 * ol. l tiT *pi. SAL. ikii. l 100 te. *tu tol, 

26.6 ' "''' <*> TUl 

i^ 31.1 *je> <",; '<r f |i|.f, 

20 3.1 . 7 aS <*-* 7 <|6.i 

2$ 3U.O 5 i. 1 ?", i7.R 

30 354 SS il.V lew r,, u<) 



IK THE SYSTRN fr>TASsnw SII,FAT, Hooxtm 

CXJ AT j^,f. 



d.of 8,u fls. ptr 
solution 

1*1862 3.64 n.n.H ii.ii ^K./^ 

1.2680 4?7 17 c 9 I0**'t * ** 

1.38^6 10.75 18.84 J^.l ' ( K r *i> 

1,4870 14. u iR.w ^.ni " 

1.4882 31.84 o.tu ^.^1 Kj, * 4 

1.4803 32.86 v, ji>.i. KH.) .!Uii * N.iJIU>4.'H r O 

1*4x36 9.56 1,6*1 $fluBK '* " 

1.4760 3.1 a KDJ **;jii " ** 

1.5800 3*54 t*H 6o.n) KH^ 4 ,H.SC) 4 .H/) * 

1.6642 4-26 2.01 ^.Ort WIS:) Ji r 4C) *'K4ll;^0 JLSO 

1.^806. s*40 i.o^ Hn.TJ " 

1.9360 9.10 Cu?j H^.riM 



or PoiAsinfM SuLfAti rn 
or HYDKOOIH Ptoxxtt AT j^ 4 e . 

d TUreit, itim.l 



WC. 
In AO. 



863 KALIUM 

SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM 
CHLORIDE, BROMIDE, AND IODIDE. 

(Blarez, i8yi.) 

Interpolated from the original results. 





Grams 1C 


ijssSO* per TOO cc. 


in Aq. 


Grams Halogen 




Solutions of: 




Salt per 100 
cc. Solution. 


In 


KHr 


K? 




at 12.5. 


al 14- 


at u.5*. 





9-9 


10.16 


9-9 


2 


3-3 


9-1 


9-2 


4 


7.0 


8-2 


8. 4 


6 


5-7 


7-4 


7-7 


8 


4.6 


6.6 


7.2 


10 


3-5 


6.0 


6.6 


12 




S-S 


6.0 



SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS SOLUTIONS OF FUTASMUM 

IlYDROXIDK AT 2,5. 
(D'Ansaiul Schrciner, lyio.) 



Mols. per 


1000 Cms'. 


Onus, per 


100 Cms. 


Mols, jmr 1000 


(Jnis. 


Gm 


X |WT 10tJ (JH 


Sat. Solution. 




Sat. St 


tlutioM. 


Sat. SolutH 


in. 


Sit SnluUun 


'(KOII)j. 


K 8 S0 4 . 


K 


OIL 


K 2 SO<. 




.OH) a . 


K 


,S< 4 . 


"Toll, 


k .-s< V 





0.6l7 


O 




10.75 


2, 


.86 


0.035 


32 


,00 


o 6 1 


0.258 


0-433 


2 


.8()2 


7.544 


3 


.42 


O,OO9 3^.33 


o , 1 6 


0-433 


0.280 


4 


.854 


4.878 


4 


.809 


O 




S3 


s> 


o 




0.137 


12 


,6 7 


2.386 

















SOLUBILITY DATA FOR THE RECIPROCAL SALT FAIR 
KtSQ 4 + BaCOj*"* K f COj + BaSO 4 . 

(Meycrholler, 1905.) 

Cms. per 100 Oms. Grm, m-r 100 (tm.s, 

t. Sat.^Sol. Solitl Phase. f. ^^J^t^^ s iH-! It4-r 

K 2 SO 4 . K a C'O 3 . K a SO 4 K,t't, 

25 10.76 o K|S0 4 +taiSO 4 25 o.6oj 7-35 w* 'o, } IUM 4 

25 6.76 5.85 " " 25 0.173 2.85 

25 3.92 12.6 " 4< 80 0.613 2,49 

25 2.485 17.81 M M +BaCQ, 80 1,39 4 ,HH 

25 1.72 22,1 K t SO+BaCO l 80 7.1 15, 33 } Ks n 

25 0.0886 28.5 " " IOO 0.797 2.36 Hftt'0 4 f IUS(I 

25 0.023 S3 -i " +K,CO,.IV> loo 1,83 4.51 " 

25 O 53.2 KtCQi.aHWHBttCO, IOO 9.42 13,6 " t K : SO, 

SOLUBILITY OF THK THREE HVUKATKS OF FOTASHIIIM Ki 
IN WATER AT DIFFERENT TKMi'ttKAit!!<h:i. 

tkUhUrr and 1'hkl, iHyy.j 
KsSO 4 .FeSO 4 .6H-/ > Ky*< ) 4 .1-VSC ) 4 .4 f \>J > , K .,S< > 4 I-V 



t. 


cc.N/ioKMnO* 


CJnts 


K 8 M), 


4 tt.N/m 


KMn(> 4 




K a sn 4 o 


,\/m 


KM 


;ni4iiiiiv 


IWMUMMI^ 




Solution. 


XOO fl 


.Sol. 


Sihr 




IOJ U 


-.Sol. 


Lluii. 


.n. 


I MK t | | 


. s,a * 


0.5 


12-4 


18 


36 


1C 5 


5 


22 , 


94 


S 


4 




7'j 


17.2 


17.0 


25 


.16 


18 


. i 


26, 


79 


,i 





3! 


t|H 


40.1 


24.8 


3^ 


-72 


21 





3^- 


.41 


;? 7 


(i 


40 


86 


60 


29.0 


42^ 


93 


24 


. i 


35- 


.68 


a 8 


,H 


42 


fi| 


80 


30.6 


45 


,29 


2/ 


.3 


40 


.46 


a 8 


6 


4J 


34 


90 








29 


.6 


43 


,82 


:>H 


9 


4J 


73 


95 


... 






29 


.8 


44, 


.11 


27 


7 


41 


-Of 



KALIUM 36/4 

SOLUBILITY op POTASSIUM SULFATE IN AQUEOUS SOLUTIONS 
OF MAGNESIUM SULFATI AH VICE VKRSA AT 25. 
(van Kiwsttr, toi7.) 

Cms, per roo Cms. Sat. Sol. ^!^ ^ phwe 

* MgSO,. K 8 S0 4 . MgSCV K,S0 4 . "* 

26.76 O Mg$0.7H f O 13.26 10.34 

26.67 1.68 " ' 12. 88 10.51 

26.57 2.34 " " 68 10.70 

26.36 3.76 " 12. 06 10.77 

26 30 4.. O2 " "HMgK a (S04)tH/> 10,69 10.84 " 

* v x>y T o 

18.76 7.02 MgK 3 (S04)|.6HjO 7* XX. IO " 

16.36 8.43 " 4 ".03 

14.27 9.63 " o 10.77 

SOLUBILITY OF MAGNESIUM SULFATE IN AQUEOUS SOLUTIONS OF POTASSIUM 

SULFATK AT 30 AND VICE VKRSA. |W<um, IMS.) 

(iim.portOOgrau, x 

jH.oB H.'9 MgS0 4 .KSO*.6H,0 

i 3. 19 11,66 

ii. SB 1-1.47 

9.49 rjt.O] K|S0 4 

3.4^ n .98 

26. o5 6.93 o.<8 u?o 

The author also gives data for the quaternary system stgitM K 1 so t -+'(N % iit,8o,>H 1 o. 

EQUILIBRIUM IN THE SYSTEM MAGNESIUM SULPATK, POTASSIUM SULFATK 
AND WATER AT VARIOUS TEMPERATURES. I Lvl, 

Gmi. per lOOnrnis. i<ti. tot 





t'i MgS0 4 . K a 80*. 

o.o... 21.09 S.i'i 

19.8... 25.34 3.83 Mx80 t ,7tt,o H- 41.7... 

a(>.i... 26.45 4.u6 19-6... 

3;.8... 29.80 4.13 ^ V5.-A... 

o 8.73 7.8(1 K,S0 4 *H 63.4... 

20,4 .. i^,.o8 lo, 10 -t- 

1.1.0 BBS Schoitlto, MgS() ( .K|80 t . 011,0; 4.1.4 L*mil% Mg HO^KyHOtU H,O. 

The author coasidert that the results of Van dor Hoide art lEoorraet, due to 
incomplete saturation. The errors in the data of others ar alto pointed out. 

SOLUBILITY or POTASSIUM NAHNSSIUM Stri.KArt IN VATSR. 



(tea. K f Mg(ao <l ) p ptr 

100 gwfi. H J3 PhM r ioo 



o iij.i K ? S0 4 .M|SO <| ,6H f O 115 40.5 

20 35.0 " 60 50. i 

30 30. a M 75 ijr>,ft 

100 gms. HO dissolve 3 o. 52 gms. ILMg<80 4 ),,6H.Q at i 
(Lothian, 1909.) 



865 

EQUILIBRIUM IN THE SYSTEM POTASSIUM SULPATB, MAGNESIUM 

SULPATE AND WATER AT VARIOUS TEMPERATURES. 



KALIUM 



d.of 


Gtas. per 100 ggi 


a. sat. sol. Soil a 


sac. sol. 


'M g so 4 


V~? PhM<s 


Results at o 


{Benrath & Benrath, 


1930.) 


1.025 


0.0 


6.68 K ? SD 4 


1.061 


1.26 


7.0? " 


1.108 


4.17 


7-51 


1.115 


4-59 


7.77 " + 1.1,6 


1. 163 


8.60 


7.85 1.1.6 


1.165 


8.94 


7-53 " 


1.192 


11.79 


6,7$ " 


1.265 


20.78 


3.03 " t MgS0 4 . 7 H,0 


1.271 


20.74 


7*93* MgSO 7H ? 


1.274 


20.68 


4-34* " 


1.259 


20.94 


2.17 " 


1.236 


20.82 


0.0 tf 


Results at 25 


(Benrath & Benrath, 


1929( A) ) 


1.088 


0.0 


10.75 K f^4 


1.123 


2.60 


10.86 " 


1.149 


5.05 


10.8$ 


1.230 


12.61 


10.99 " * \.i.6 


1.249 


14.28 


9.89 1.1.6 


1.267 


17.02 


9.18 " 


1.294 


20.32 


7,32 


1.347 


26.02 


4.90 " t HgSC) 4 .?H % 


1.324 


26.61 


2.11 MgS0 4 .7Jf^O 


1.305 


26.65 


o.o w 


Results at 30 


(in terms of guts, per 100 gm. H ? 0) (Si.trni ind Clark f 






1010. 1 





0.0 


11*11 K^SO 





4.80 


14.24 " 





12.03 


15.26 '* 





16.04 


15.32 M 


"" 


17.72 


1S-31 " 1.1,6 





18.51 


14*45 1,1.6 





26.17 


l i . 39 " 





31.78 


8.89 





37.43 


7.19 M 





39-91 


6SS H * MgS0 4 * 7H f O 





39.13 


5.53 MgS0 4 -7H f O 


*~ 


39.29 


S79 w 


- 


39.10 


0.0 ff 



1.1.6 I SchOnite, K g S0 4 .MgS0 4 .6H 0. 



Bozza, 193^, also gives a compilation with diagrams of all available 
data upon this system at temperatures between oand 10,0 calculated to 
the terms proposed by Janecke. 



KAliUM 

POTASSIUM SULFATE 



866 



EQUILIBRIUM IN THK SYSTEM POTASSIUM SULFATE, MAGNESIUM 

SULPATE AND WATER AT VARIOUS TEMPERATURES. (Continued. ) 



Una. per 100 



LJ 



sat. sol. 


/ Mg8Q 4 


K f^4 


Results at 35 


(Rozza, 1934, ) 




1.148 


5.0q 


12*40 





7.16 


12.28 


1.242 


13.13 


11.67 


1.250 


14.40 


11 .90 





16.15 


10-20 


1.283 


17.82 


9-33 


1.284 


20.37 


7-55 





2'}. 60 


5.6l 


1.360 


28.45 


4.35 


1.336 


28.41 


1.78 


1.332 


29.20 


0.0 


Results at 50 


(Renrath and Ben-rath, 


1929( a) ) 


1,087 


0.0 


14.14 


1.148 


5-05 


14.13 


1.255 


13-86 


13-47 


1.292 


16.96 


13.10 


1.290 


17.36 


13.06 


1.322 


21.83 


10.32 


1.337 


24.39 


8.14 


1.370 


28; 59 


5.98 


1.394 


32.35 


4.30 


1.380 


32.76 


2.60 


1.383 


33.50 


0.0 


Results at 66 


(Benrath and Sicnelschmidt , 1931.) 


_ 


0.0 


16.16 





7.73 


15.01 





14.01 


14.37 





17.08 


14.46 





19.33 


13.04 





26.97 


7.67 





32,53 


5.86 





33.89 


4.48 





35-66 


4.01 





35,4.0 


2.08 



Solid 
Phaae 



1.1.6 



1.1.6 



" + MgS0 4 .7H ? 
MgS0 4 . 7 H ? 4 



11 + MgS0..6HJ) 
MgS0 4 .6H ? 4 



35.52 



0.0 



" + MgSO..H ? 
MgS0 4 .H ? 



1.1.6 = Schonite K 



1.1.2 = K p S0 4 -MgS0 4 .aH p O (Leonite). 



86? KALIUM 

EQUILIBRIUM IN THE SYSTEM POTASSIWM SlTLPATB, MANBSEIIM 
SULFATB AND WATER AT VARIOUS TEMPERATURES. (Continued.) 



d Of 


Otaa. pr 100 jni 


sal. sol. 


A Mjao 4 


Results at 75 


(Benrath and Sichel 


1.095 


0.0 


1.151 


8.51 


1.225 


12.70 


1.302 


17.18 


1.320 


l8. 12 


1-351 


23.32 


1.402 


26 . 44 


1.419 


30-70 


1.421 


31.66 


1.424 


32.13 


1.449 


35-50 


1.437 


3S.23 


1.435 


37.11 


1.432 


37 . 30 


Results at 85 


(Starrs and Storok, 





6.08 





13.60 





17. *n 


- 


19*97 





24*66 





27.74 





32.01 


. 


33.9 


1.1.2 r K. SO 


.M R SO .2\\ (Loon it 


1.1.4 = K-SO .>' 


tgSO ,r|H,,0. 



17.05 K,,S0 4 

16.13 
15-70 
15.22 
10.00 

11.14 

8.70 

7,71 

4.41 

4 2 
2. 30 
1.25 
0.0 



17.71 
I 6 . 911 
in. 86 

17*16 

6.58 

"\ . 27 
tl,C) 



H TUB SYSTFM PoTAfisrM S 
Sur.FATK AND WATER AT too . 
(Benrath and Benrath, 1930.1 <Sr,vrr:i .ind Sturt.:k, 





d 


.of 


Oms. per tOO pi*. 


i'tai. 


ptr 100 


iff*. 


aat. 


a at. 


solution 

^^.MMMM. 




>Ul1 


aat. 


. ulutlurt 


sol. / "~~ 


Mg80 4 K ? n 


r * h 


itat / HI 


io 4 




,;< 


1 


. 


119 





. 





19- 


42 K p S0 4 


O 


.0 




19, 


1 


. 


217 


7 


. 


30 


19. 


n6 " 


H 


. f * i 




i >, ^ 


1 


. 


339 


16 


. 


25 


18. 


75* " 


l*J 


6n 




i v ! < 









18 


. 


00 


18. 


84* " 


17 


*i"i 




1 H ! < 


1 


. 


30$ 


14 


, 


47 


18. 


64 " t 


1.2 n 


75^ 


21.91 


I^.c 


1 


. 


304 


18 


. 


12 


14. 


26 1.2 


16 


*49 




l. * 


1 





319 


22 


. 


63 


9. 


04 " 


20 


.71 




1 . i, 


1 


. 


332 


27 


. 


44 


"> 


54 " 


^5 


.60 




6, 


1 


. 


361 


31 


, 


00 


3 


31 " * 


MfifSO JfJ) jc> 


,yo( 


v*u) 


1 . i 


1 





367 


33 


. 


27 


0. 


o MgSO 


H-0 ' 11 


.7^f 







'>1M 
"hAf 



*'* 



o> "* \'.'tfVH,;> 

H|jM) 4 ,f? f ;1 * 



* Metastable 

This system was also studied by Campbell, I)own* 4n4 S,ur*, p M ,,, 
their results give a curve which dif fercon*udcr*ibly trim th.it *f 
Benrath and of Starrs and Storck. Their v,ilu/s.s for fh^ triph ptii 

are shown in parentheses. 



KALIUM 868 

Data are given for the reciprocal salt pair K f SO + MgtNO ) * 
K ? (N0 3 ) ? at o and 995 Bearath and Bearath, 1930; at as^'&nd^o 
Ben rath and Benrath, 1929*; at 75, Bearath and Sichelschmidt, 1011 ' 

Data for the system K g S0 4 + MgS0 4 + NH 4 ),S0 4 * H p O at 30 , calcui aled 
from the results of Weston, 1922. are given by Jlnecke, 1937, iQ ^a 

Data for the system K ? S0 4 + Mg$0 f KCl * HgCl f + II ? Q at 100 are 
given by Campbell, Downes, and Samis, 



SOLUBILITY or POTASSIUM SOLFATI IN AQUEOUS SOLUTIONS 
OF MAMGAHISI SULFATI AWO Vici VBRSA AT o. 

(Cavwi ami Johnston. 1917.) 



(tea. per 100 iM ^ ac - 0l* Itolidi (to a. pr 100 m. sat. !, 

' ^ --^--^ p ^^ / .,-..,^^,.. ,.,,..., . .,,. ^ 

4 l> 4 4 t^4 

o.o 6.82 K F S0 4 37*62 4.48 

6.21 7*7$ H 10.38 4.00 

8.21 7.97 " 14-30 VT5 

11.80 8.48 " 14. 18 3.8l 

13.68 8.88 " * MnSO .KjS0 4 .4fi f O 34,53 1,85 

17*39 7.60 MaSQ 4 . K^SC^.i&Hj/) 14*49 1.68 

23.64 S54 M 34.78 o.oo 
25 SO 5 * oo " 

EQUILIBRIUM IH TH SITSTIM POTASSIUM SLrATi t MAKGAIIBSB 
AHB WATIR AT VARIOUS 



0*s. pr tOO p. fls*. pw 100 . 

aau oolnrinn lia 



17.5 


14.85 


10.85 


K S 


D 4 * Mas 


66 


8,63 


16.75 


I ^ 


30 


15.46 


12.2$ 





* 1.1.4 


IK 


1 l.")5 


14,77 


1.3 


n 


33.64 


5.50 


1.1 


4 * 1.3 


80 


0*0 


17.92 


K.SG 


35 


15.65 


13.10 


K f S 


4 *1,1.3 


* 


3*l8 


18,60 


w ** 




30.40 


6.6 


i.i 


.4 * 1.3 


H 


S41 


18.40 


tl 


40 


14*26 


13.78 


KtS 


04 * 1.1.2 


n 


5.84 


18.40 


M * 




27.18 


7.22 


1.3 


4, w 


H 




i* 


A 


w 


34.66 


3*34 


N 


+ Mai 


tf 


6^92 


IV 80 




50 


0,0 


14.17 


K t S 




,. 


8^81 


io8a 


* 




2.77 


15*02 


M 




fl 


14.57 


6.66 


n 




7.36 


15.11 


If 




M 


16.65 


6*19 


* 


H 


11.78 


15.34 


W 


4 i.i.a 


ft 


20,42 


4.8$ 


w 




14*43 


13.40 


1.1 


.2 


M 


39- SS 


3.61 


tt ^, 




16.45 


12.34 


n 




ft 


30*24 


0.0 


Mm 




17.17 


11.85 


H 




97 


0.0 






N 


18.30 


11.55 


ti 






209 


id 9 8 


^w "* 


n 


18.70 


11*41 


n 


* 1.3 


n 


1.63 


19.89 


H 




21.52 


9.51 


1*2 




w 


4. OS 


16*84 


t2 




24.82 


7.30 


it 




it 


4*)1 


13. SO 


tt 




37.9 


5.85 


n 




w 


$.46 


9-68 


H 




35.22 


3.49 





* Mm 


M 


7.08 


7. as 


It 




37.3 


0.0 


Mm 




* 


11.65 


6*00 


tt 


55 


10.50 


15.91 


K S( 


X * 1.1.3 


Wi 


17.0 




* 


H 


16.71 


12.83 


1.2 


4, w 





35.93 


3*48 


W ^ 




33.6 


3*1 





* Moi 


ft 


38.49 


o.o 


Mm 



1.1.3 



1.2 



i.a 



Mai 



869 KALIUM ] 

SOLUBILITY OF MANGANESE SULFATE IN AQUEOUS SOLUTIONS OF 
POTASSIUM SULFATE AT 5 AND VICE VERSA. (Cavon and Johnston, t20.) 
Gms. per 100 ms. Gms. per i<W gms. 

sat. sol. 8 l - ol 

MnS0 4 . K,SO V 

89.10 o.o 

3 9 . 03 0.43 

38.54 1-87 

38.42 2.46 

38.21 3.o3 

37.92 4-i5 

37 .28 4 20 



Solid Phase. 


MnS0 4 . 


K 8 S0 4 . 


Solid Ph. 


JVJnS0 4 .4H 2 


35.58 


4.3o 


1.1.4 





3o.47 


5.27 





*> 


19.27 


10.06 








16.58 


1 2 . 3 1 


+K t SO 





1 5 . 22 


12.04 


K 2 SO & 


-4-1.1.4 


6.36 


n .^ 





1. 1. 4 


0.00 


1 2 . 59 






... 

SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS AMMONIA SOLUTIONS ATSJG. 

(Girard, 1885.) 

Cms. NH 8 per 100 cc. solution o 6.086 15.37 24 . 69 31.02 
Gms. K 2 S0 4 per 100 cc. solution 10 . 80 4.10 o . 83 0.14 o . 64 

One liter sat. solution in water contains 105.7 gma. KiSCX at 20. 
One liter sat. solution in 5.2% NH* contains 45.2 gms. KaSO* at 20. 



EQUILIBRIUM IN' THE SYSTEM AMMONIUM SULFATE + POTASSIUM 

SULFATE + WATER. (Wetton, 1932.) 
Results at $5. Results at 30*. 

Gms. per 100 gms. Gram, per 100 gms. 

sat. sol. Solid Pbaid. 




(NH,) t S0 4 . 

o.o 43.5 

1.83 40.9 

3.09 38.6 

4.00 37.0 

4.40 35.1 

5.42 3i.4 

7.35 22.3 

9.52 10.7 
10,70 o.o 

The solid phase at both temperatures consists of a continuous n<ri<Mi of mixed 
crystals. The author also gives complete data for th quartornary system 
(NH 4 ) a S0 4 + Mg S0 4 + K 2 S0 4 + H t 0. The results aw axpnmaad in terms 0! 
the H a required for the solution of roo gm. quantities of various mixtures of the 
three salts. 

SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM SULFATE AND AMMONIUM 

SULFATE AT 25. 

(Pock, 1897.) 




Grains j>er Liter. 


Milligram Mols. per Liter. 


Mol. per cent Sp. Or. 

KA 4 { f 


Mc4, per emt 


KaS0 4 . 


(NH^aSO,. 


KaSQi. 


(NHtbSCV ' 


Ml/4 in tn 
S<uuticm. Solutton. 


KSO 4 in 

Solid 1'hue, 


127.9 


o.o 


734 


0.0 


IOO 


,086 


IOO 


135-7 


"5-7 


778.5 


874-6 


47-x 


.149 


91,28 


84.20 


281.1 


483 


2126 


I8. 5 


.200 


So, os 


59-28 


355-0 


340 


2685 




.226 


68.63 


40-27 


482.7 


231 


3<% 


S'9 


.246 


2 7S3 


o.oo 


542-3 


o.o 


4100 


o.oo 


245 


0,00 



Results are also given for 14, 15, 16, 30, 46, and 47. 



K KALIUM R 7" 

BQUILIBRIUM IN THI vSysiiM POTASSIUM SULFATB, 
AMMONIUM SULFATK AND WATEE AT o AH? AT so . 



tesults at o 




Resul is at so a 




In. Mol. Prcii 


ta. Hols. H ? tu 


'to. no I. l*rcni 


ta. MoU. H to 


(NH 4 ) ? S0 4 in 


dlstolvtt IOQ P- 


ff4H 4^? ; - W 4 ll1 


aioiv too IPS. 


fed K ? S0 4 * fHH 4 ) f S0 4 


Hal, salt aiuur* 


UiMOlVttU K IV) * fNH 4 t,SO 


Hois. Salt mixture 


100 


IOO 


IOO 


75 


90 


130 


90 


8S 


80 


iB< s 


80 


100 


70 


2 r iO 


70 


120 


60 


us 


60 


us 


SO 


W :i 


so 


780 





l ifki 





S3S 



The solid phases consist of A aerie* of mixul cryst.il-i containing the 
two salts in a continuous ratio. 

The author also gives results for tho qtsariernary systems in ihe re- 
ciprocal salt pair K f S0 4 * aNH S0 4 * * aKNO, - tN[L>^\ a , 2S a & 

50. Similar data for the recspnical salt pair [K f ^" 4 ) ? 1 C^^ 4f CrOp 
at 25 are given by Ishikawa, 11926.1 

SOLUBILITY OF POTASSIUM SUI.FATK IN AQUKDUS SOLUTIONS OF SODIUM 

SULFATK. 
SO 

Results at 25, Result s at 34** and at (xf 

(Smith and Ball, 1917.) (Nitkrn, ino.) 

Clm.H, per 100 Gms. Cms, per 100 <m*- Clnts IHT 100 t'Jnw, r r , 

H/). Sut. Sol. at t,$". \t Sl ,it V M . Stijiil I nav ^ 

At ;I4 4fi< a,l 60 . 



o 12.05 o n .(> o 15,3 KSO, 

1.78 12.33 7.1 10.7 6.6 !.<. 9 " -HilanrrUe 

3.58 12.6$ 31.4 4.3 27,1 8,2 N*t*0 i' Mix r rystals 

5.38 12,89 33.1 % 31.3 O N^S0 4 

7.19 13.0 

Additional data for the a'>ove systein at 15*. 25, 40*, 50**, <*f* 70* antl Ho* 1 are 
given by Okada (19x4^. The results ahow that (xttawitttn and wKlium sulfates 
form a double wit of the comfxwitton KNa(S()4)s. Thii* dfiiitile salt titMolvM 
sodium sulfate as a solid solution but not potassium sulfate. 

I^QUILIBEIUM IN THK SYSTEM PoTAMU'M St,:i,l''4TK, SciIJIUM Sl'M'ATK AND VVATEH. 

Constant stirring for about ,{o lint, nt v** mui 10 !iri. at yo win employed. 



TJio nbov<i: ri'tttiUs ut '^,1 an* taken from MeyerhoflW in*l HattnlTi*, 



871 



KALIUM 



POTASSIUM SULFATE 



EQUILIBRIUM IN THE SYSTEM POTASSIUM SULFATE, AMMONIUM 
SULPATE AND WATBR AT VARIOUS TEMPERATURES- 

(Bovalini and Pabrl, 19?.) 



Qs. per 100 gws. 
at. solution 



Results at -3.3* 
6.802 6.201 

Results at -13.63* 
a. 448 30.54 

Results at -17.82* 
2.568 36.46 

Results at -18.76* 
1.447 38.29 

Results at o 



6.513 



6.010 

5.245 

4.790 

925 



2.928 
2.688 
2.431 
0.852 

Results 



11.80 
9.651 
9.072 
7.134 
5-468 
3.860 
2.191 
0.698 



7.222 
12.894 
18.98 
25-23 
30.71 
31.69 
35-21 
36.99 
38.82 
40.90 

35 

5-450 
13.42 
19.41 
28.50 
34.32 
38.60 

42.22 
43.30 



4t. <?, K ? S0 4 1ft Mlxisd 


(to*, ptr 100 |p*. Wt. * K ? 4 Us HUU 


Crystals composing 


sat. conation Crystals composing 


Solid Phase 


'lOso"*"* *""""""* 'NlTj JQ? aolld Ptiut 

? 4 4'P 4 




Results at 50 


95.6 


13.27 6.09 9^.9 




10.05 19.67 89,6 




7.5 29.06 8l.6 




6.09 35-54 70.9 


83.15 


5.49 36.35 64. a 




4.41 39.91 40*0 




3.652 40*03 n*< 




0.790 45.23 * 


33*9 


0.580 45.49 1.6 




Results at 70 


6.32 


16. 0(| 4.58 o*, 7 




14.61 9,64 )7> 




11.98 20.01 o;.;t 




9. 28 27.65 BJI.H 


99.1 


7.149 34.14 7!. ? i 


97.8 


5*06l 39*49 53-n 


96.1 


3.33 41,21 V-H 


90. l 


1.19 45.66 n.i 


72.8 




71.6 


Results at, t>6.<5 


32.7 


17.56 11. Ha *H.6 


11.6 


9*59 32,30 6y.; 


5.1 


7.04 19-21 U7.H 




Reault at io;i.6 a IU.pt. S 


99*5 


17.10 12.63 H6.3 


89.1 




80,9 


Result at 106.7 <b.pi. I 


72.3 




63.6 


8,62 37.31 49. a 


54.1 




26.0 


Reault 41 107,2 (b.pu) 


5. a 





Congealing temperature with ice. 



K KALIUM 



872 

SOLUBILITY OF POTASSIUM SUI.PATE IK Aarmotis SOLUTIONS 
op SODIUM SULFATI AT 25 AND VICE VIRSA. 

n na 8*1 Uu XQJO.) 



0m. pr 100 *B*. 



V4 



0.0 12.05 

2.842 12.485 

5.684 12.943 

7.92 12.33 

10.63 11.37 



27.75 o.o 

29.574 1*486 

31.633 6.759 

32.53 8.288 



SO 



EQUILIBRIUM IH THE SYSTEM POTASSIUH SULFATE, SOD inn 

SULFAT AKD WATIR AT VARIOUS TBMPIKATUKBS. 
(Cormc tod KrwaUtieh. \%m* 19 .} 



r 


a. of 


c 


s&t. sol. 





1.120 


1.8 


1.120 


10 


1.160 


n 


1.128 


20 


1.228 


" 


1.139 


28 


1.314 


ti 


1.144 


30.9 


1.363 


34.0 


1-3S7 


50 


1.339 


n 


1.157 


75 


1.322 


" 


1.167 


100 


1315 


It 


1.173 



fisny. per 100 



5.26 

9.75 

$40 

17.34 

5. Si 

26,36 



solution 



7.75 
7.8 
7.53 
8.09 

6.94 

49 



PttMt 



Gl 



Naio 



Naio 



31.07 


4.80 


30.73 


5.03 


29*40 


1.8s 


5-68 


13.77 


27.84 


7.18 


5.64 


16.43 


26.97 


9* IS 


5.52 


18.80 



4 Na 

4 w 

* KLS 

* Na 

* Na 



Na = NaL,S0 4 ; Naio = Na^SO^iol^O; Gl = Glaaeriie; 3K f ^ 

double salt capable of dissolviag N* f 8G 4 but not K^SD to form solid 
solutions (mixed crystals) with a filiation in content of K f 8G 4 from 
78,6 to 61.8 percent. 



These authors also give data for 



in water, including densi- 



ties, of potassium and sodium sulfates and nitrates at so to 90 

Complete experimental data for equilibrium in aqueous tola t ions of 
mixtures of potassium and sodium sul fates, nitrates And chlorides (in- 
cluding densities! at temperatures between o aael 90** are given by Oon<ec 
and Krombach, 1929 and Gomec, Krombach aad %ack, 1910. These authors 
have made use, whenever necessary, of the results for ternary and quaternary 
systems previously reported from their own laboratory or by others, includ- 
ing Cretien, 1929; Cornec and Hering, 1925-7; Cornee &ad Kroftbaeh 1929! 
Meyerhoffer and Saunders, 1899; dAns 191 j and Blasdale, 1918- 

Data for the system K^S0 4 * Ma ? SO * K f C 
are given by Teeple, 1929. 



873 

EQUILIBRIUM IN THI SYSTEM POTASSIUM SULFATE, NICKBL 
SULFATK AND WAT1R AT DIFFERENT TSMPgRATURKS. 

(Benratii, 193?.) 



KAL1UM 



On s. per 100 
gns. sat. ao 1. 



Solid 
Phase 



Ctas. pr 100 

tpaa. aat. sol. 
__-a_ 



o 6.8o 0.14 KgS0 4 "*" 1.1.6 40 2.08 

11 1.09 21.62 NiS0 4 .7H 25 Oi.i.6s5 14.76 

25 1.18 29.52 " " M 2.30 

30 1.30 32.4 " "* 88 2.99 

NiSO-.6H_Q<x 100 20.21 

r/N * - 



40 13.15 0.51 KySU 4 * 1.1.6 

1.1.6 = K ? S0 4 .NiSQ 4 .6H g O 



33-35 NiS0 4 .6H * K K 6 

1,2 K SO* * Li.6 
35.0 N1SO*.6H^* 1.1.6 
41.19 " H 
5.19 K SO + i.u6 



3.60 42.3 N!S0 4 .6H/>$+ 1.1.6 



SOLUBILITV OF MIXTURES OF POTASSIUM AND LEAD SULFATES AND OF 
POTASSIUM AND STRONTIUM SULFATES IN WATER, 

(Barre, 1909.) 
Results for K 2 S0 4 + PbS0 4 . Results for KaSOi + SrS0 4 . 



f. 


Cms. K|SO< 
per 100 Cms. 


Solid Phase. t\ 


Cms. KfSOu 
I^er 100 Gmi, 




Sat. Sol. 




Sat, Sol. 


7 


0.56 


PbS0 4 .K 8 S0 4 17.5 


1.27 


17 


O.62 


4 Q 


1.88 


So 


1.09 


75 


2.71 


75 


1 -37 


IOO 


3-90 


100 


1.69 


" 





K,SO 4 .Sr.SO 4 -fSrSOi 



EQUILIBRIUM in THB SYSTIM POTASSIUM SULFATI, 

SULFATI AND WATER AT 25. 



Qns. per 100 ana. 
sac. aol. 



Solid 




~ 4.07 S^^-^I^J^iyo 0.32 0.88 3K f S0 4 .Pr f <80 J,.aH r O 

4.01 " * 0,40 0.67 sK.SO. .aPr-(S6.L,8H0 

3.20 4^KS0 4 .Pr J> (SO ) 3 0.52 0.34 

0.18 i".o 3 3^SO^.Pr*(SOj)*!4p 3 - 6 3 0^19 ** 4 " r *_' 4 *' a * 



SOLUBIHTY OF POTASSIUM SuLFATE IN AQUEOUS SOLUTIONS OF XlNC Stf|,rATB 

AND VICE VERSA AT 23. (Cvi and Jobnuton, tw. I 



Gins, per J 00 .gins, 
mt. sol. 




S(.H<I 

K S so, 
>* 

K,SO<.%n$0 4 .A!f,0 



25 . i r 



.c5 

.'H'I 

44 



,B.oi 
JM.5H 

!!( , CKI 



Hothi 



K KALIUM 



874 



SO 



EyiULIBRIOM IK THE SYSTEM POTASSIUM SlTLFATE, 7.1VC 
SOLPATB AND WATER AT VARIOUS TEMPERATURES. 

19SO.) 



Qas. p 
t gs. aa 


er 100 

[,. SOl. 




Solid 


Omsi. p 

L pan. sal 

f- f - A 


r 100 

. Ml. ^^ 


' 2nS0 4 


w 






4 


K ? B0 4 ' Ph M 


0.0 


6.88 


K SO 


1.1.6 


BO 27-10 


10.26 1.1.6 


" 3.68 


2.91 


1.1.6 




" 31.00 


B.60 


11 29.83 

12 0.37 

" 32.60 


0.99 
9.69 
1.82 


1.1.6 
K,SO 

1.1.0 


+ 7,nSO .7^0 

* 1. 1.6 
7,nS0 4 .7iLO 


" 36.84 
" 38.38 
" ^8,63 


6.51 
6.6g " * XnS0 4 . 
6.02 ZnSO . H^O 


41 3.18 
" 40.30 


13.78 
2.50 


K 2 SO 
1.1.6 


1.1.6 

ZnSO .6H f O 


11 38.92 

" 40.56 


0.0 " 


50 4.34 
" 43.20 
68 39.90 


14.28 

2.15 
4.20 


1.1,0 


1.1.8 

ZnSO .6HJ) 
ZnS0 4 .H ? 6 


160 o.o 

11 9-0(5 
" 10.l6 


19.42 K ? 80 4 

20.50 " 

21.41 " 


80 o.o 


17.55 


K p SQ 




11 3J.18 


20,07 " * 1.1,6 


" 2.07 


17.87 


H 




11 24.96 


l 9 , H 1,1.6 


11 8.48 


18.17 


ti 




" 24.40 


lB.85 


" 11.80 


18.24 


it 




" 25. 83 


17.69 " 


" 13.46 


17.77 


ii 




rt ^o.6a 


15,08 


11 13.67 
" 14.32 


18.14 
16.91 


1.1.6 


1.1.6 


M 16.70 

" ^6. 9^ 


n.ji " XnSO . 
7.H 7,nS0 4 .H0 4 


" 16.29 


14.36 


n 




w 3B.85 


a. 21 


" 21.04 


13.15 


" 




t. 1?w7l 


. " 


" 23.00 


12.17 


" 









1.1.6 = K,S0 4 .ZBS0 4 .6H | ,0. 



SOLUBILITY op POTASSIUM SULFATI IN Agtutous SC>L'TIOHS OF 
URAKTL SULPATK AMD VICE VmnA AT j^, 
(Coiani, w.) 



Solid 

HtJUH' 



Gna. ptr 
ant. sc 


100 tpa. 
>|uuon 


0.0 


10.40 


0.91 


10.67 


1.59 


11.02 


2.39 


11.17 


2.41 


9.01 


2.43 


7.31 


4.73 


3.50 


9.91 


2.69 



DMU ptr 


100 UPS. 


r gg- - 


liuUmi 

K^80 . 


31,69 


1.91 


35-07 


1.79 


19-73 


1.77 


51.70 


0.71 


59-30 
61.50 
6l.2S 
61.18 


0.54 
0.45 
0.21 
0.0 



JJ80- 



UO p S0 4 .3H f 



875 KAL1UM 

SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS ALCOHOL. 

(Gerardin, 1865; SehiiT, i86j.) 

In Aq. Alcohol of 0.939 * n Alcohol of Different 

Sp. Gr. = 40 Wt. %. Strengths at 15. 



to 


Gms. KSO,i per 100 


Weight per 


Gms. K 8 SO| per 100 


. 


Cms. Alcohol. 


cent Alcohol. 


Gnw. Sat. Sol, 


40 


0.16 


IO 


3-90 


80 


0.21 


20 


I .46 


60 


0.92 


3 


o . 56 






40 


0.21 



SOLUBILITY OF POTASSKW SULFATK IN AQUEOUS ALCOHOL AT 25. 

(Fox and Clause, ryto.) 

Gms. per 100 Cms. Sat. Solution. Gws. per roo Gms, Sat, Solution. 

^K 2 S0 4 CjjHjjOH. H 5 0. ' R.SO 4 . l'HOH. HO 

9.17 1.35 89.48 2.6(> 15.26 82.08 

6.90 4.80 88.30 1.83 20.50 77,67 

4.96 7.80 87.24 0.07 26.01 72,12 

4.32 9.70 85.98 0.41 35.07 (*j.(>i 

3.57 12.34 84.09 0.22 43.00 55.88 

2.71 14.51 82.78 0.016 69.26 30.72 

SOLUBILITY OF POTASSIUM SULFATE AT 25 (Fox ami 'augr, XM.) IN: 

Aqueous Chloral Hydrate Solutions. Aqueous Glyivrol Solutions. 

Gms. per 100 Gms. Sat. Solution. Grm. j>t*r 100 (rnf. N.tt Solution. 



K 2 S0 4 . 


CClaCH(OH)j. 11,0. 


' k 


-so,. cr 


H.uilt 


sCiro 


II, it. 


,n 


9 


-13 


6.44 


8 4 . 


43 


8 


.87 


8, 


.06 


82 


,17 


8 


.41 


9-00 


82. 


SO 


7 


.60 


13 


36 


78 




7 


79 


".3 


79- 


83 


6 


.47 


20 


-34 


73 


.10 


7 


3i 


13 . 20 


79. 


49 


S 


83 


24, 


15 


70 


,02 


5 


.88 


22.O7 


72. 


5 


4 


.44 


33 


73 




,Hj 


4 


54 


33 15 


62. 


31 


3 


.65 


40 


.40 


SS 


OS 


3 


36 


44.40 


52. 


24 


3 


38 


43' 


5"5 
** 


53 




2 


.92 


47-30 


49. 


78 


2 


.69 


50 


.l8 


47 


'3 


2 




62.82 


35- 


18 


2 


.07 


57 


2 2 


40 


,71 


I 


75 


70.28 


27. 


97 


1 


53 


67 


.04 






I 


.40 


80 . 36 


x8. 


24 





.98 






20 


,84 


I 


.08 


85.26 


13- 


66 


O 


73 


98, 


,28 


o 


. 00 


SOLUBILITY OF POTASSIUM 


SULFATE 


AT 


25 (Poxi 


me) Gautft% it 


MO.) IN: 






Aqueous 


Acetone Solutions. 


Aqueous 


Pyridlne Solution*. 




Gms. p 


ioo Gms. Sat. 


Solution. 






(*rn. prr 


*OG CJmi, Sat 


, Solution. 




K 


2 S0 4 . 


(CHa),CO. 


HA r K,S() 4 . CH<(i:H,('U), 


>N. II, 




7 


.20 


4-9 2 


8 7 . 


88 


7 


95 


4, 


,23 


8 7 . 


.82 


5 


.02 


10. 06 


8 4 . 


02 


4 


,77 


13, 


90 




1$ 


2 


.96 


16.23 


80. 


8r 




75 


24, 


5* 


72, 


74 


I 


50 


24.31 


74- 


K) 


T 


.47 


34 . 


1C) 






0.47 


3/.IQ 


62. 


3-t 


o 


45 


46, 


2C) 


S3 


26 


O 


.20 


46.29 


S3- 


5* 


o 




55" 


03 




05 


o 


.03 


62.40 


37- 


57 


o 


,006 


75- 


,90 


24 , 


,09 



K KAL1UM 



876 



SO 



SOLUBILITY OF POTASSIUM SULFATE AT 25 (Fox and Gauge, 1910.) IN: 
Aqueous Ethylene Glycol Solutions. Aqueous Mannitol Solutions. 

Gms. per ioo Gms. Sat. Solution. CJms. per roo Gm^ Sat. Solution. 



1,804. 


(CH 2 OH) a . 


H 2 0. 


^ K S SQ<. (CHOH) 4 (CH 2 OH) 


* HW>T* 


9.67 


3.16 


87.17 


10.32 


3.20 


86.48 


7.69 


9-79 


82.53 


9.61 


8-35 


82.04 


5-74 


i8.47 


75-79 


9.19 


11.26 


79-55 


3-57 


32.11 


64.32 


8.66 


14-3 


77.04 


1.83 


49 -3 


49.14 


8-35 


17.22 


74-43 



SOLUBILITY OF POTASSIUM SULFATE AT 25 IN: 

ucrose Solutions. Aq. Potassium Ace 

and Gauge, 1910.) (Fox, i& 

Gms. per ioo Gms. Sat. Solution. Gma. per xoo Gms. Sat. Solution. 



HfTso, 


___. .A.-.. 

CH a Oi,. 


H 2 0. 


'"lEiS04 


CHiCOOK. 


H 9 0. 


Q 65 


9-S 6 


80.79 


6.65 


6. II 


87.24 


8.65 


18.55 


72.80 


5'09 


8.68 


86.23 


7.42 


28.16 


64-42 


3-99 


11.29 


84.72 


6-35 


37-24 


56.41 


2- 35 


^5-59 


82.06 


5.21 


47-55 


47.24 


1-23 


20.12 


78.65 


4,24 


57 


38.76 


0-39 


29.95 


69.66 



ioo gms. ;?lycerol of J- 1. 255 dissolve 1.31 6 gms. KiSCXat ord. temp. <Voel, 1867.) 

SOLUBILITY OF POTASSIUM SULFATE IN AQUEOUS ACETIC ACID AND IN 
AQUEOUS PHENOL SOLUTIONS AT 25. 

(Rothmund and Wilamore, 1902.) 

In Aq. Acetic Acid. In Aq. Phenol. 

Moh. iyr Liter. Grams per Ota*. McK per Liter. Cirumn per Liter. 



(jCQQ HL. K.2SO4. CHsCOOH. k*SO. H|OH. Kjt&tV 


cv'i 


ftOH. 


K8S04. 


O-O 


0.6714 


o 


o 


117 


.0 


o-o 


o 


.6714 


o 


.0 


II7.0 


0.07 


0.6619 


4 


.2 


115 


4 


0.032 


o 


.6598 


3 


.01 


115.0 


0-137 


0-6559 


8 


.22 


114 


4 


0-064 


o 


.6502 


6 


02 


"3-3 


0-328 


0,6350 


19 


.68 


110 


.8 


0.127 


o 


.6310 


ii 


94 


IIO-0 


0-578 


0.0097 


34 


.68 


106 


-3 


0-236 


o 


.6042 


22 


.19 


105.3 


I.I5I 


-5S5 6 


69 


.06 


96 


.87 


0.308 


o 


.5834 


28 


97 


101.7 


2.183 


o4743 


128, 


-58 


82 


.70 


0.409 


o 


.5572 


38 


,46 


97-2 














0.464 


o 


.5480 


43 


.Ql 


95 -5 



0.498 (sat) 0.5377 46-82 93.8 

ioo gms. water dissolve 10.4 gms. KaSCX 4- 219 gms. sugar at 31.25, or ioo 
gms. sat. solution contain 3.18 pjms. KsSGi -f- 66,74 gms. ugar. (Kdhkr, i&97-) 
ioo gms. 95% formic acid dissolve 36.5 gms, KtSG* at 2i . (Ajchan, 19x3.) 
ioo gms. 95% formic acid dissolve 14.6 gms. KHSO< at 19.3. " 

ioo cc. anhydrous hydrazine dissolve 5 gms. KgSO4 at room temp. 

(Webh and Broderson, 1915.) 
ioo gms. hydroxylamine dissolve 3.5 gms, KtS04 at I7-I8 . (dc Bruyn, 189*.) 



877 

SOLUBILITY OF POTASSIUM SULFATB IN AQOIOUS SOLUTIONS 
OP MBTHYL ALCOHOL AT 25. 

(AJcerlof and Turcic, 1935.) 



KALiUM K 



Wu Percent 
CH 3 OH in 
Aq. Solvent 

0.0 

9.7 
15-09 
21.30 



Oka. Mola. K g SO 
per 1000 S. 
Aq. Solvent 

0.6905 
0.3049 
0.1933 
0.1134 



Wt. percent 

CH.,OH In 

AQ. Solvent 

29.99 
40.10 
59-94 



per 1000 was. 
AQ. Solvent 

0.0536 
0.0321 
0.00342 



SOLUBILITY OP POTASSIUM SULPATB IN AQUEOUS ETHYL ALCOHOL. 

(Wright, 19FM 



20 
100 



Wt. Percent C,pH OH 
In Aq. Solvent 

50.0 
50.0 



a. AQ. Solvent 

0.14 

0.51 



SO 



SOLUBILITY OF POTASSIUM SULPATI iw AQUBOUS SOLUTIONS 
OF VARIOUS COMPOUNDS AT 25 

(Weber. 191*9.) 

da. Mola, JCJ*> 4 per liter In Aj. Solution oft 
Aqueous Solution of: " t 

Water alone 
Cane Sugar 
Manni te 
Methyl Alcohol 
Acetonitrile 
Ethyl Alcohol 
Acetone 

Methyl Acetate 
Propyl Alcohol 
Methyl Ethyl Ketone 
Diethyl Amine 
Phenol 
Aniline 
Par aldehyde 
Ethyl Acetate 
Butyric Acid 
Ter. Ainyl Alcohol 
Valerianic Acid 
Iso Amyl Alcohol 
Hexyl Alcohol 

d) - 0.2 Normality instead of 0.25; (3) = 0,185 Normality instead of 
0.25; (3) = 0.0208 Normality instead of 0.125; (4) = 0.0416 Normality 
instead of 0.25. 



TfTlfiTTo maXnoT" 


"ITTiSnRoTiiniyv. 


WSSHW". 


nr^rwiinrv 


0.5562 


0.5562 


0.SS62 


0.5562 


0-5537 


0.5555 


0.5532 


Q 9 S43iO 


0.5518 


0.5538 


0.5496 


* S 4 311 




0.5295 


0.5000 


04$t 


0.5398 


0.5359 


0.4381 


0.4313 


0.5356 


0.5187 


0.4783 


0.40^3 


0.5313 


0.5086 


0,4574 


0.3827 


0.5408 


0.5349 


0,4938 


0.4336 


0.53H 


0.5068 


0.4577 


0386l 


0.5308 


O.S030 


0*4S4S 


0*3744 


0.5293 


0.5040 


0.4633 


0*3663 


0.5291 


0.5030 


0.4556 


*- 


0.5224 


0,5079 U> 


. 


MM 


0.5229 


0.4931 


0.438? 


"*" 


0.536S 


0.5186 


0.4828 





0.5410 


0.5292 


0.50SS 


0*46lS 


0.5178 


0.4797 


o.iM'O 


03153 


0.5393 


0.5236 


- * 


*. 


0.5158 


0.5065 (a) 





~" 


0.5476 (3) 


0.5407 (4) 









KALIUH 

SOLUBILITY OP POTASSIUM SITLFATI IN AQUBOUS SOLUTIONS 
op ETHYLINB GLYCOL AT 30. 

(Triabl, 1931.) 



a. of 


Gas. pr 100 m 


s. sac. sol. 


d. of 


(tea. pr 100 


^s. sat. aol, 


sac. sol. 


/ ~CH^OHCH ? OH 


K ? S0 4 ^ 


MU aol. 


^OHCym 


K? 80 *^ 


1.0881 


0-0 


11.14 


1,0646 


38.S8 


2,q.l 


1.0812 


4.21 


9.84 


1,0708 


49- 7S 


1.4S 


1.0737 


9.01 


8.11 


1.0823 


65.62 


0.63 


1.0651 


18.64 


S-66 


1. 1060 


100.00 


0.00 


1.0627 


28.91 


3.67 









SOLUBILITY OP POTASSIUM SOLFATB IN AQUEOUS SOLUTIONS OF URETHAN AT 25. 

(PalltBtch, iQ?e. 19W.) 
Orn. MOU. ptr 1000 pis. HjD 8oU<l 



0.690 0.0 K^SO^ 

0.468 1,1235 " 

0.026 23.49 " 

0.0l6 50.45 " 

SOLUBILITY OF SOME POTASSIUM DOUBLE SULPATES IN WATER AT 25. 

(Locke, iyoa.) 
Double Salt. Formula. 'iSrw^mH^ 

Potassium Cobalt Sulfate KjCo(S0 4 )2.61IaO 12*88 

Copper " K t Cu(S0 4 )i.6HiO 1 1 . 60 

Nickel " K 8 Ni(S0 4 )2.6H0 6.88 

Zinc " KaZn(S0 4 )i.6HjO 13.19 

SOLUBILITY OF POTASSIUM NICKEL SULFATE AND ALSO OF POTASSIUM ZINC 
SULFATE IN WATEE, EACH SEPARATELY DETERMINED AT DIFFERENT TEM- 
PERATURES. 

Gm. per xoo Gms. H g O. Cms, per 100 (ims. IT/). 



.6H S 0. .6HaO. .611,0. . 

o 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 

SOLUBILITY OF POTASSIUM NICOL SULFATI in 



(tea. Kj,Nl(00 4 ) ptr Solid Ot*. K^HH80 4 ) f pr Solid 

UK) gas. *&&. sol. Phaoo c ;oo tpa. aac. wl. 



o 3.26 K^Ni(S0 4 ) ? .6H 40 8.97 K F Ni(S0 4 )^6H g O 

10 4.31 ' 11.02 M 

!5 4.93 " 60 1333 " 

20 5.6l " 70 15.88 " 

2$ 6.36 " 80 l8.68 " 

30 7.1? " 90 21.74 " 

ioo 25.04 M 



8 79 KALIUM 

100 gms H sat. with Potassium Neodymium Sulfate, KNd<S0 4 ) p .H ? 0, 
contain 1.7 gm. KNd(S0 4 ) g at o and 1.3 gms. at 20. (Meyer and 
Kittlemann, 1931 * 

One liter sat. solution of Potassium Zinc SuHate in Water contains 
85.94 gms. K^Zn(S0 4 ) ? at 6.8. (Haber-Chuwis, 1926.) 

Fusion-point data are given for the following mixtures: 



K g S0 4 
KHSO, 



Na6l 3 
NaJSO, 



(Kendall and Landon, 1920; Camhi and Bozza, 1933.) 
(Camhi and Bozza, 1923.) 
( Amadori, 1913. ) 
( Bowen , i 926 . ) 
(Sackur, 1911-12.) 

& w (Janecke, 1908; Nacken, 1907 (bMc); Sackur, 1911-13.) 
Rb5l 4 (Dombrovskaya, i933*J 
Rb SO " " 

+ Sr0/ (Grahmann, 1913; Calcagni, 1912, 1912*-* 
POTASSIUM Ethyl SULFATE K((\IU)S(). 

SOLUBILITY IN WATKR. 

(Illingworth and Uowurd, 1884.) 

Cms. K(CiH|)SOi 

t*. pt 100 Gms. 

Sat, Sol. 

-14.2 45-01 

o 53 7 1 

+ 15 63.JS 

SOLUBIIJTY OF POTASSIUM IVFIIYL SUI.KATK, POTASSIUM MKTHYL S^ILFATK 
OF POTASSIUM AMVL SUIJ-ATE IN WATKK, DKTKEMINEU HY THK Kui 



SI 



POINT METHOD. 

Results for K(QIlft)SO 4 
-f 11*0. 

* . Gm. 

Solid 

Phase. 



i awl l 



I, IH.|.) 



Results for K(CH 3 )hU 4 
4- IW). 

Solid 



Results for K(C"fe!Iy)SC)4 

+ H 3 CX 

,J"$y- K(C.'{?,1)S0 4 SolM 



catlon ' Gms.Sul. taiwn ' CJnw.Sol. t MMU (Imn. Swl 

2.2 ID Ice 2.3 1O Ice 1,0 IO Ice 
~ 4-9 20 " - 3,6 15 " - 4.3 ao 

- 8.2 30 " - s 20 " - 5-4 J4 

r 2. 1 40 " H 30 " -4 

14.2 45.01 "+K((VI : ,)S0 4 -- n .H 30,84 " +K(n!)SO 4 4.8 as K 

6 50 K((' 9 Hfjsc> 4 1 1. 5 40 K(CH])SC)t o 3,1-44 
o 53.71 " o 47,1 " 'i- i 7,3 59.40 

+ 15 62.35 (t +12.3 54.8 

100 ipns. methyl adcohol dissolve 1.73 gms. Batnasiuw ethyl s 
at 15 and 13.87 g*ns. at the b. pt. {65,8). (Hens lock, 19311.) 
SOLUBILITY OF POTASSIOM ETHYL SULPATE ii MIITOIIS or 
METHYL ALCOHOL AHB ACBTOIE AT 20. 



The results are given only in the form of & diagram from which the 
following approximate values were read* 



Percent Acetone 
In Mixed Solvent 



o 

10 
20 
30 
40 



per 100 



Solvent 



2*2 

a. $5 

2*8 
2. 95 
2.8 



Percent Ace urn e 

in H1K4 aolvtti, 

60 
70 
80 
90 



ptr 100 



3. as 
i. 75 

i. as 

0,70 
0,0 



KALIUM 880 

POTASSIUM Ethyl SULFATE KC S H 8 .S0 4 * and p forms. 
SOLUBILITY OF POTASSIUM ETHYL SULFATE IN WATER. ( Hammu-k ami Muliaby, 1921.) 
This compound is dimorphous. On crystallizing from methyl alcohol or water 
there first appear tufts of long feathery crystals which redissolve as the solution 
cools and give place to the ordinary foliated form. Analysis showed no difference 
in composition between the two forms. The temperatures were determined at 
which the edges of crystals, present in synthetic mixtures contained in sealed 
tubes, changed from rounded to sharp or vice versa. No matter at what tempe- 
rature crystallization occurred the unstable $ form was always the first to separate. 
It was easy to distinguish which solid phase was present at the different tempe- 
ratures. The transition point was found to be at 5l.B. The ice curve was deter- 
mined by the freezing-point method. 

J D r t" of solution for 

Cms. KC a H 4 S0 4 per ^~~- l *+^**-**~---~** <Jm, KC S US0 4 per 

t*. 100 fins. uat. sol. Solid Phase. &> form. p form, too gms. sat. sol. 

1.195 5.48o Ice 4.5 13.5 49-5 

i.i4* 6.37 1.9 5i.g46 

2.i3o.. 9.434 -+-8.7 5.2 58.8i 

2.98 12.953 *i.o t 12.1 66.6 

3.2'i 18.770 *>6.o 20.1 70.015 

4.93 19.808 35.o 32.0 75.'icj 

6.68 a5.c/>3 -HM) 38. 'i 77.99 

9.55 33.714 4^.5 45.0 80.084 

vi . 9 ieuiec.1 . . : . r a form 5j,i4 5r.i 8a.o4 

I5.i - ! P 59.4(l 84.44 

65.8 85.47 

69.1 86.*.3 
8 % i. 3 87.9.1 

91.2 89 . 62 

POTASSIUM N-Phcnyl 3 A-mino Ethyl Hydrogen SULFATE C,H,NH.CH 4 . 

O.S0 3 .K. 

100 cc. sat. sol. of the above compound in water contain 3.o grns. C G HNH. 
C 2 H 4 .OS0 3 .K at 1 5. (Sauntiw*. \m.) 

POTASSIUM I>henyl SULFATB, C S H 8 4 SK, etc, 

SOLUBILITY OF EACH SEPARATELY IN WATER AND ALCOHOL. 
(Burkhurdt and lapw^rth, 10i@. ) 

(iiM. cinpd. 
Compound. Formula. Solvent. t" prlMftns, H^O. 

Potassium phenyl sulfate. C 6 !l ft 4 SK Water 17 16.28 

Alcohol 17 0.704 

m carboxy phenyl sulfate. C ? H|O ft SK Water 17 3.*>, 

anaphthvl . CioH 7 QtSK 17 a. 5 

p CtoH 7 O4SK.4l( s O 17 *.{'} 

POTASSIUM PerSUUfATl KtStO. 

SOLUBILITY IN WATBE. 

(Tarugi, 1904.) 

t . Gms, KsSjOi per t Cms. KiSA per * Gm, KAOi per 

1 * 100 cc. Sat. Sol. * 100 cc. Sat. Sot. * zoo cc. Sat. Sol 

o 1.620 15 3.140(3.7) 30 7.i9o(7-7) 

5 2.156 20 4.490 35 8.540 

10 2.600 25 5.840 40 9,800 

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 HSOi liberated, according to the equation KaS-A-j-HiQ 
K 4 S04 -I- H 2 S04 -f O. Tarugp also reports that the presence of a number of 
sodium and other salts in solution, does not appreciably alter the solubility of 
K^SjiOs in water. 

100 gms. H 2 dissolve 1.77 gms. KsSsOs at o*. (Marshall, 1891.) 



88 l KALIUH 

SOLUBILITY OF POTASSIUM PERSULFATB IN SATURATED AQUEOUS SALT 
SOLUTIONS AT 12. 

(Pajetta, 1906.) 



(An excess of the salt and of K^SaOs was, in each case, added to water and the 
mixture stirred at constant temperature for 10 to 20 hours.) 

c- 1* Gms. KaSfOg per c,i* Gnw. KjSjOg per 

Salt ioo Gms. Sat. Sol. ** tt ' ioo (Jim. Sat, Sol. 

Water alone 3 . 196 KaS0 4 o . 798 

Na 2 S04.ioH 2 O 6.238 KHSO 4 0.336 

NaHS0 4 8.842 KNOa 0.004 

Na 2 HP0 4 .i2H 2 4-766 KjCO 0,0146 

Na 2 B 4 7 .ioH 2 3-^5 KHCO a 0.317 

NaN0 3 19-302 MgSO 4 .7HsO 2,900 

Na 2 C0 8 .ioH 2 O 5.682 CaS(>4.3Hs(y 3-3% 

NaHCOa 5-42 

Additional determinations made with salt solutions of lower concentrations 
than saturation, gave the following results at 12,5. 

Gms. Salt per Grra. K^O,, Cms. Salt jwr Citm. KtSO, 

Salt. ioo Gms. ixjr joo Gms. Salt. ioo (iirw. JHT ioo Gms. 

H 8 0. Sat. Sol. H f O. Sat. Sol, 

Na 2 COb 2 . 304 4.297 NaHSCX 5.218 4 , $ 56 

NaHCOa 3-652 4.230 NaNOs 3-M 4.613 

Na 2 S0 4 .ioH 2 7 4-554 NaJHPO* 3.086 4^446 
POTASSIUM THIOSULFATE K 2 S|0 3 . 

SOLUBILITY IN WATER, (Jo, i9xxx9ia,) 

Gms. KaSjOs (ims. K|^() 3 

t. per ioo Gms. Solid Phase. t a , per ioo limn. Solid Phjwe. 

H a O. 11,0, 

O 96.1 K a SA. 2 H a O 56.1 234.5 

17 150.5 3K a SA,sH s O 60 238.3 

20 155.4 " 65 245.8 

25 165 ' 70 255.2 

30 175.7 " 75 268 

35 2O2.4 " "fKtStOa.HaO 78.3 2C)2 

40 2O4 . 7 KtSaOa-HiO 80 2Q3 , 1 

45 2o8 -6 " 85 298.5 

50 215.2 " 90 312 ** 

55 227.7 

POTASSIUM Sodium TmOSULF ATI KNaSi0..aHjO. 

ioo gms. HaO dissolve 213.7 gms. KNaStOi.sHtO (a) at 15, (Hchwkkvr 
ioo gms. H 2 dissolve 205.3 gms. KNaStOf.aHjO (b) at 15, 

POTASSIUM THIONATES 



or BACH SEPARATIST XN WATIR. 

(Reaulco for Hi th ion ate t>y deBaac. ig^e; for Uio uUuirfl Oy KurtonocRor M4 



" 100 nr. f&, 
,_, ^ "fi'jipj 



'K DiThioiurw~~**T TrithioftAw" K ^TmSTooSc5'~""TtT ii toM 



K Ve SVe K A fl VA f - l -' f H r o) 

o 2.52 8.14 X2*6o 15-50 

12 4.28 

20 6.23 18.43 33.18 a<*78 

30 8.54 - 



K KALIUH 882 



POTASSIUM THIONATES 



EQUILIBRIUM IN THE SYSTEM POTASSIUM TRITHIONATK, 
POTASSIUM TBTRATHXONATR AND WATER. 

fKurttnacK.tr ana Fiuaa, w^\ ) 



tsns. par wo A; 
t r-j^fc 

o 6.68 

20 1.80 
2.30 

6.86 
11 11*50 
" 13.26 

EQUILIBRIUM 


fLi'ASi. i: itolld ** ptr lw? 

^P S 4f "* PIiBJIt l ^ K^ii ' '"" 

12.00 ^^4^ fl 4> K ? ^5^ f JO 14.^1 

21.85 Ko^ 4 0. * ' M 16.70 
21.60 " ' " 16.3, 

18.82 " ' 17.67 
18.90 " " 6.68 

18.65 ft * K ? S 5 0^ 

IN THE SYSTEM pnTAsnM FKTRATHIONATR, 

PFINTATHIONATE AND VATRR. 

^KurunacKr ar*i Fluaa, to^*^, > 


f* a - aa h,, 8oh soiiu 

K ?* S 46 "*' p fM 

14.17 K S^O 

11.94 tl?? 6 

S.75 " 

1 2 . 00 " 

POTASSIUM 

is. su sol. Solid 
"Vv/V ^ Phaat 

!). K 'g S 4 ( V 

14.10 " 

8,70 

POTASSIUM 
9.9H K.S^S 

1.74 " ' " 

4*17 " 
2 . 46 " 


o ^. 71 14.49 KpS^+K^O^iA^pao HKH 

20 2.53 21.39 K p SO f .iili;o ' " u . 71 
S.86 20.59 " * " 114. , 
" 7 S3 20.19 " " 17.39 
" 10.34 20.86 " 1 8. 01 
11 10.88 20.10 " + VV^ " ,uu*{6 

EQUILIBRIUM IN THE SYSTKM POTASSIUM TRITHIONATB, 
PENTATHIONATE AND WATER. 

(Koirtcae,ir and Flus, low, ) 


7.6 
20 6.35 


7 3D K S (V 1 4 II * t) 4. *"? ll 
rfU * *T J. \/_ . 1 S II g^J V O lll Oil 



High accuracy is not claimed for the above rcsiiltn since the pnly- 
thionates begin to decompose after short peri oil.* of sli 



KALSUM 



POTASSIUM SELEHITE K ? SeOj,.5H p U. 

SOLUBILITY OF POTASSIUM SELINSTE IN WATEK. 



d. of 

sat. sol. 



0.262 
0.50 
0.97 
2.375 
03 



- 5 

-13-0 

-23.6 



-20,5 

- 9.7 

- 0-2 

MO. 5 

13.5 

19.5 

24.3 

o 

20.3 
43.1 
60. i 



(Butec. 



100.6 

* Metastablc 



1.007 
1.015 

1 . 029 
l . 07 5 



1.282 



(tr.pt,) 



100 



1 . 02 

2.02 

\ 99 

9.S4 

17. $7 

32.01 



6 1 . i a 

rt2.7f 

6<. i \ 
65.81 
67.00 
68. S 

68.45* 
68.48* 
A8.S3 
6R.70 

6B.51 



* K.SeO , 



POTASSIUM RiSELBNXTR 
POTASSIUM PytX)9BLBNITR 



SOLUBILITY or POTASSIUM BISELINITI ANI PYOSILINIT, IN WATI. 



s&u sol. 



100 



o. 166 


1.003 


0,6^ 


0.365 


1.010 


l.S^S 


0.694 


1.023 


3.09 


1.342 


1.047 


6 . on 


3.17 


1. 119 


14. 12 


6.285 


1.237 


25.55 


14.3 


1.466 


41. 11 


'22.7 


1.6055 


S2. *^ 


57-0(7) 





70.01?) 


20.6 





71*52 


"10-5 





74.29 


0.2 





75.87 



,'iotid 



too 



Ice 


l j*8 


77.31 


tt 


1 8 . <) 


78. 18 


It 


31,0 


78.70 


It 


as ^ 


79.11* 


M 


^0.6 


80.04* 


11 


ait. 


79ot? 


tt 


27.^ 


79*21 


" * KHSteO 


*,(>* 4 


Ho . it) 


KHSH),, ' 


69.6 


Ba4S 


i 


90.8 


H i . 7 .\ 


i. 


102-8 


84,47 



PtiMt 



* Metastable 



K KALJUM 

POTASSIUM Tetra SELEWITE 



SOUJBILITf OP POTASSIOM TlTiA SlLIHXTi W WATER. 
a, 1032; Jftniciu* MO ouuMnttu* um.} 





a. of 


QM. XX-fgtOg) 


c 


sau eol. 


100 *t. 


D.ir/8 
0.288 


1*003 
1.009 


0,59 
1*467 


0,544 

1.027 


1*040 


a. 905 
5.69 


2.302 


1.102 


*343 


'4*10 


1.203 


24. 6a 


7.42 

8.0 


1.399 


43.3 
46,0- 



Solia 



-6,9 46.53 KH (SeQ, ) 

0.0 53.S7 3 " 3R 

Hi, 9 63,20 " 

20.3 68,6$ H 

31*0 7S7a 

50.8 8s*55 H 

S94 ^9.65 " 



POTASSIUM SBLENAT! K t SeO. 

SULUHILITV IN 

t*. "^". C- 

Cms. KiSc04 per 100 gms. solution 51^5 51.7 

. 



52 52.6 54.9 



., - 

ioo gms. HjO dissolve 115 gins, KjSeOi *it ii'. (Tmttm, 190?,) 

More receat deterwl nation a by Htyer 4nd Ayiieh, i*>a8 A&d Friend, 1929, 
fail to agree md a satisfAciory explAa*iion o{ ihr differeoce is not 
apparent. Although Friead eplyetl 4 perioti of nh4king of only a hours 
and Meyer and Aulich, 4 10 6" hour* his reftttUs are ilie higher. The fol- 
lowing values were taken fnw AverAgi^ cttte^ drawn fron th^ original 
results in the two casts, 



on, 



^^ V** 1 * ^ fr 
mr A lulichp 



-20 Si5 *o Sl^^t 54.15 

5^*8 i*5^ 50 5.$05 54.4 

10 52*2 51.51 60 Stt.l 54.7 

20 Sa6 5I7 70 5H-51 55.0 

25 52*85 51. H 85 M!.H; SS*6 

30 si.l 5i>5 ^W) 55. tt 56*2 



TM1 

AND AT 



Omu. por 100 j^id, MU Mi,, telia tlkii, pit* IttO . in%, iL 
,-. ''Hp^"""^ phi f ^^| "'*#* "^ 

S33 o.o ^*^*^ 4 jui i,iio 1,1 .6 

lUnH 
u.*iw 
I I* i? 



50.58 


0*63 


H 


l)*V r * 


47.31 


0.89 


w *i.l,6 


1<I.1*> 


38.50 


3*13 


l . 1 .6 


S*Sa 


30*24 


S44 


N 


o.o 



1.1.6 = 



885 KAUUM K 

EQUILIBRIUM IN THE SYSTEM POTASSIUM SILENATE, SODIUM 
SBLSNATB AND WATER AT 25* 

(Meytr ana Aullch, 1928.) 



(tots, per 100 


gas. sat. aol. 


Solid 


Gtea. pr 100 


0. oat. sol. 


Solid 


r K 2 Se 4 


m ? so 4 ~T 


Phase 


^ " u * ?! 5So 4 


Ra^tO.""^ 


Phase 


53-3 


0.0 


K 2 Se0 4 


23,24 


38.52 


K g Se0 4 


45.20 


7.21 


" 


21.86 


31.29 


11 * Na ? Sc 


37.72 


12.76 


If 


19.87 


31.78 


2 4 


30.02 


19.90 


II 


17.42 


32.34 


H 


26.80 


35.36 


l 


Q.O 


36-40 


II 



POTASSIUM Neodymium SELEftATE KNd{$e0 4 ) t . i*H Q. 

100 gms. H p O sat. with KNd(Se0 4 ^.^G contain 15.0 gms. KNd(Se0 4 ) |{ 
at o and 25.0 gms. at 20. (Meyer and Kittletnaan, 1931.) 

s in 

POTASSIUM SILICATfe K,SiO 3 . 

Data for equilibrium in the systems K^Si() 3 -f H a O, KsSi)0 4- H 4 f KSiO s -f 
Si0 2 , SiOa + HaO and K 2 SiG 3 + SiOj 4" HO, at (cm|Xiratrc8 between imf and 
1000 4- f determined by the " hydrothcrmal quenching incthml," are given by 
Morey (1917)- 

POTASSIUM STANNATE K 2 Sn0 3 .3l! 3 O. 

100 gms. HjO dissolve 106.6 gnis, at xo, and 110.5 gms. at 20**. Sp, Gr. at 
IO = I.6l8 at 20 1.627. ' (Ordway, t6,;v) 

POTASSIUM STANNATE K,Sn(OH)and K s Sfi(()Hj n ,aiI a (), 

SOLUBILITY OF THE ANHYDROUS AND THE HYDRATKD SALT, EAC:II SEP A HATKLY, 

IN WATER. ( %ochr, ttiao. i 



t". P 

*H ....... , ......... fa.? K 2 SiH..OII) f 

>.a ........ ...... ... 5-J! . 4 KiSiuOHh.-4H.jn 

POTASSIUM TELLURATI K,TcO 4 . 

100 gms. HaO dissolve 8,82 gms. KsTcOi at o 27,53 K ms * lt 2O *^*^ 50.42 gms, 
at 30 . (Rosenhdim Miui Wcmhbr, 

POTASSIUM VANADATE K,V*Ou.sHiO. 

loo gms. HjO dissolve 19.2 gms. at 17.5. (Rattan, 

POTASSIUM ZINC VANADATE KZnV*Ou.8HtO, 
100 gms, HaO dissolve 0.41 gm. of the salt (Kadun). 



POTASSIUM TUNOSTATE K f W3 4 

Fusion-point data are given for the following mixtures. 



Licmpt, 
(Van Lictnpt, 1922; Hoermann^ 



Kr KRYPTON 

KEYPTON Kr. 



886 



SOLUBILITY OF KIIYPTON IN WATI-.H, 

The following now <lrl<Mrmiuu(i<us \\viv iual in ; 

* '* 



\utru|MiiT, 



The following new df.tvrmiuutioiis \\viv made, in a^ rolmod apparatus arranged 
so that the solvent and it vapor touched no i'w*k. Tin* JHVVIOUH doiurminations 
were found to bo in error in the rogitm of tlu minimum. Tin* roMull.s are expressed 
in terms of the Bunsen coellifirnt ..as modified by Ku<nm, that IK the volume of 
gas in ee. (reduced to normal condition*] dissolved by i.o %m. of lf a (,). 



t ". Alworp. eorffi 

o o.i ro r > 

io o.oHio 



, cocf. 
0.0357 



The above determinations have been rtrc.ilcul.urd by V,Ufntiner, i<>27 

and expressed in terms of the OstWAld Soluttilify ' which is thi rela- 
tion of the concentration of th^* gas in the li juid to the gas phase and, 
According to the Henry-Dai ton law, is indtpond*i oi the parti dl pressure 
of the gases at a given temperature. 



o 
10 

20 



or 

U 05 

0.0840 

0.0671 



60 
70 
80 



a 

0.0418 

0.0403 
0.0398 



KRYPTON Kr 



SOLUBILITY or KRYPTON IN SKVIKAI. I lytims, 
BY SIHPLX MKTRADS TO AN ACOUMM y or ABOUT 



Results of K6rAsy 1937 
Soivuat t* 



Ethyl Alcohol (<>$%) 

(97. 5> 
Cyclohexanol 

Acetone (technical) 

H (dried) 
Benzene 
Tetraline , 

Butyl acetate dechn. ) 
Butyl phth&late " 
Tricresyl phosphate " 
Acetic acid (glacial ) 
Glycerol 

Chloroform 
M 

Bromoform 

Carbon tetrachloride 

Aq,. 20% CaCl Solution 
Ar in Chloroform 



of V.w lt|n and Van tfijk, 1937 



21 0,^2 


W.urr 


a.5 


0,12 


Jl 0*6? 


H 


ao 


o * 06 


23 O.IICI 


CiAJitilint' {flrn?,iiit) 


i> 


0,89 


19 0,H< 


Pi*irol*ui 


;o 


1,00 


JO !.OJ 


Paraf f tn* oi 1 


iH.s 


0.6 o 


2J 0<>7 


Bt*ft x**ti* 


19 


0.67 


ait o4*i 


Toluene 


iH 


0,84 


30 O.HS 


Methyl alcohol 


18 


o.sa 


30 0,U7 


Riliyl rt f*iCiti 


1*1 


O.^i 


aa oai 


%l 


J'l 


0,66 


22 0.7 


Glycirol 1 tool) 


JJ 


o.oi 



30 O06 

o 0.97 ^ = <"<: Kr iat o and 760*01.) 

ji KI rli.Hsoi vi*tl by i,occ solvent 

o ujo of Kr an <\ vapwr of :u>lv*nt. 

21 u ;l i 

22 0*014 The Krypton ut*d to tu^th ca.ie;* 

23 0,178 coniAin*ii about s |>f*rciiU of xeoon, 



Data for the solubility of Krypton in liquid Oxygen nf* givn by 

v. Stackelberg, 



LANTHANUM L, 

SOLUBILITY OF LANTHANUM IN MERCURY. 

(Parks ana Campanula., 1930.) 

Analgams of lanthanum and mercury were prepared by heating the mixed 
constituents in fused quartz flasks to 200" or by electrolysis of 
Lanthanum Salts dissolved in absolute ethyl alcohol, with Hj is the 
cathode. Such amalgams were kept in evacuated fused quartz flasks at 
the selected temperatures, approaching equilibrium from above and below, 
A filtered portion of the saturated solution was allowed to stand in con- 
tact with the air until the lanthanum had separated <ts the hydroxide .utd 
this was then determined by titration. 

Q QHU$, La pr <ta*. La ptr 

c too am- La 4 H L 100 tPu Ln * Hg 

O.OOSS2 37 5 o.oi 14 

12.5 0.00907 $0.0 0.018*1 

2$0 0.00960 

LANTHANUM BROMATE La< BrO^ J^f^O. |^ r ( 

SOLUBILITY OF LANTHANUM BROMATS IN WATER. 

(James, Pbfg, Mcln&lrt, Evana and Donovan, 19??,) 
Ctos. ptr 100 gfa. sat. ol. Q (fcu. pr 100 jp* tat,, sol. 

49.48 64.83 20 50.83 78.40 

5 52.06 68.22 35 62.74 8-%3i 

10 S4.59 71 S3 3<J 66.63 B?.;|i 

15 57-02 74.89 35 69,74 'Jl.'jtt 

LANTHANUM ACETATE U(CH :1 C(M) i,,. |i/, H,o. 

100 gms. H^O dis>olve v.o.<(H gms. La(rj|,(!OO) :i at iH u . ! v'Mrlrjr, IHS ii7,/ 

100 gms. Methyl Alcohol dissolve 0.64 gm. L*i{CH^CCX)) at 15 dod 
0.77 gms. at 66 (b.pt.). (Henstock, 1934. I 

LANTHANUM CITRATE 2(LaCyi 6 O,),7H a Q. 

100 gms. aq. citric solution containing to grnn. citric acid per 100 ci\ diiiMolve 
0.8 gm. La(C e HO;) at 20. ' (Hotmtoi. 1907.) CII 

LANTHANUM OLYCOLAT1 La(C 2 !l 3 O 3 ) 3 . 

Oneliter H 2 dissolves 3.328 gins, l,a(CiH 3 Oa)a at 20. (Jwtsch ami timakmut, iiia-i j.) 

LANTHANUM MALONATE La,(C,HA)i.5HO. 

loogms.aq.Am.mabnatesol. (logmn. per iQOcc.)disM)lvt*o.,2 gin, ( i^i((\H s C)4)i 
loogms.aq. malonic acid 8ol.(2Ogms. per loocc.) dissolve 0,6 gin. j at Mf, 

LANTHANUM LACTATE I^:,H^) ;| ),.:UI(>. 

100 cc.. sat. solution of lanthanum lactatc* in water contain i.il mm l. u 
[ 4-o6 gms. La (C, H, C),) t .:j II, 0] at v.<. ' j Mlw ', i; 



La LANTHANUM 888 

l^JrTHANTJM TARTRATE La^C^AO^H/). 

One liter H 2 dissolves 0.059 gm. Lai(C4O<O) at 25 (solid phase * 

3HaO). Determined by electrolytic method. (Rimbach and Schubert, 1909.) 

SOLUBILITY OF LANTHANUM TARTRATE IN AQ, TARTARIC ACID AND AMMONIUM 
TARTRATB SOLUTIONS AT 20. 

(Holmberg, 1907.) 

In Aq. Tartaric Acid. In Aq. Ammonium Tartrate. 

Cms. Tartaric Acid per Cms. Lat(C 4 OA) s Pr Cms. Am. T&rtratis per Cms. L%(QH 4 0^ 8 per 

100 cc. Solvent, 100 Cms. Sat. Sol, *oo cc. Solvent. *oo Cms. Stt, Sou 

2O O.6 1O O.2 

40 1.2 20 0.6 

LANTHANUM SULFONATIS. 

SOLUBILITY OF EACH IN WATER. 

Gmf, 

Anhydrous 

Sulfonate. Formuk. Sulfonulc Authority. 

<ti per too 

' n Gin*. IM). 

Lanthanum Benzene Sulfonate L*(CHso)j.9HtO (,$ , i (Holmberg, 1907.) 

" m Nitrobenzene Sulfonate tt!CftH 4 NO|SQrii-6HiO 16 

" m Chlorbenzene Sulfonate UIQH^CLSCU^H/) 131 

m Brombenzene " U(C|HBr.S()ib.9HO i a o 



" (6) Chloro (3) Nitrobenzene ( i) {Sulfo- \ L(( < H^CKNC^SC^JaJHiC) 24 5 

" (i) Bromo (4) Nilrobenmie (2) f nate ? l*(C4H*BrNOOt)t*SHiO 5 (Kau 4 Jam, '13,) 

" a Naphthalene Sulfonate LafdASOs^H/) 5 2 (Holmberg, 1907.) 

" i . 5 Nitronaphthakne Sulfonate LatCwKtCNO^sOji^ftHsO 0.55 

" 1.6 A " a .9HO 0.21 

" 1.7 " 4i M .9i^D i.x 



LANTHANUM Cobalt iCYANIBK Ut(CoCiN f )i.9HjO. 

100 gms. aq. 10% HCl (dn - 1.05) dissolve 10.41 grns, salt at 25^. 

Cjam and Willtnd, 1916.) 

UJffTHANIJM OXALATE Lai(C^04)3,9H,O t 

or LANTHAWM OXA^ATI in WATBK AT 35. 



por 11 tor oat. ftoluUon, l>Leniln.J by; 



MUu>d MeUiOfl MUjoa 

0.00062 (Rlmbauck wd Schwbert, 1909.) 

0.00070 0.00096 o.ooiax (Hawser and Herxfeld, 1913.) 

0.00206 0*00214 ~~ iSarver awd Brinton, 1927.) 

0.00060 0.00208 0,00195 (KoHhoff jmd Elraquist, 1931.! 

Solid Phase La g (C f 4 ) s .9H f O in 4il ewes. 

loo gms. aq. 10.2% HNOt (d - 1.063) di^lve o.fk> gm. i*at(COi)i at 15. 

Cv, S<"!i<"**U* ' iH'ju } 

ioo gms. aq. 19.4% HNOt (d - 1,116} di^ive 2,69 gms. Ln 9 (CA)i at 15*. 

(V, Schcvlr, iKgt).) 

SOLUBILITY OF LANTHANUM OXALATE IN AQ. SOLUTIONS OF SULFUKIC 

ACID AT 2$\ (Hawser awl Wlrth, 1908; Wirth, 1908; Wiith, 191 a.) 
Nonnal- Omt. per ioo Gnt. Norauil- Gnw. per too Gm. 

S>t. Eol. SdklPhiie. ity 'oC __^L^L-_. SoUd Phwic. 



O.I 


i 

o 


.0208 


L% 
o, 


0346 S 'L%(Ct04)i,oJI0 * 


UA - 
0,4417 


' UtU'Ah, 
0.7344 


o.S 


0.0979 


0. 


1629 


3' 


,09 





,680 


I 1306 


i 


o, 


.2383 


o. 


3<62 


4 


32 


o 


,S8o 


t 4630 


i-S 


o, 


319 


o. 


S304 " 


S- 


.6 


I . 


.092 


I 8iSS 



889 LANTHANUM I 

SOLUBILITY OF LANTHANUM OXALATB IN AQ. SOLUTIONS OF OXALIC ACID 

AT 25. (Hauser and Wirth, 1908.) 



Cms. per zoo Cms. Sat. Sol. 



Solid Phase. 



Normality of Aq. 
Oxalic Acid. 

o.i unweighable 

i.o 0.00032 0.00053 " 

3.2 (sat.) 0.00045 0.00075 " 

Results are also given for the solubility in mixtures of sulfuric and oxalic acids, 
loo cc. aq. 20% triethylamineoxalate dissolve approx. 0.032 gm. LaaCCsOi)*. 

(Grant and James, 1917.) 

SOLUBILITY op LANTHANUM OXALATB IN AQUBOUS SOLUTIONS 
OF Acros AT 25. 

(Sarvar and Brlnton. 1027.) 



From 50 to 1000 gms. of the saturated solutions were evaporated to 
dryness in small porcelain dishes and the residue converted to oxide 
and weighed. 



Normally of Acid Ctao. L*g( c g0 4 ) 3 Pr 
In Aqueous Solvent too 0ns. aac. acl. 



of Acid (tea. UyfC^),, ptr 
in Aqueoua Solvent 100 jpi&. MC.*iol. 



o. 1008 


HC1 


0.2576 


II 


0.5004 


l 


0.978 


11 


1.0.84 


11 


2.000 


11 


2.865 


" 


4*000 


" 


5.200 


" 


0.978 


" 4. 0,1 


2.000 


" + 0.1 


2.865 


11 0.1 


3.965 


" + o.i 


0.978 


"4-0.5 


2.865 


" * 0.5 


3.965 


" 0.5 


1.484 


" sat. 


4.00 


H + sat. 



<COOH) S 



0.0208 


0.2482 HN0 3 




0.0567 


1.992 " 




o. 1384 


4.054 " 




0.3074 


2.00 " + 


0.1 


0.4937 


3.03 " 


0.1 


0.6770 


4.00 " + 


0.1 


1.082 


2.00 H + 


0-5 


1.327 


3*03 " * 


0.5 


1*285 


4.00 Mlf + 


0.S- 


0.0532 


4-00 " * 


sat. 


0.2998 


6.00 " . 


sat. 


0.6330 


0.086 H f SO^ 


^ 


1.026 


0.419 " 




0.0062 


0.958 " 




0.1098 


1.846 ft 




0.3^27 


2.612 " 





0.03S4 
0.9256 
2.66o 

o. 3908 

227 
568 



CO 



1. 

0. 

0.3576 
0.7200 
0.7664 
1.304 

0.0222 
0.1078 

0.2523 
0.5128 
0.6840 



SOLUBILITY or LANTBAKUM OXALATB IN AQUBOUS SOLUTIONS or NXTSXC ACXB 
AND IN AQDBOUS OXALIC ACID SOLUTIONS OF NITRIC Aci AT 90. 

(Neiu*r ana Krtmers, 19 WJ 

The mixtures were frequently shaken during 36 hours. For analysis 
5occ of the filtered saturated solutions were evaporated to dryness in 
porcelain dishes and the residues ignited and weighed as oxide. 



No reality of Acid 
In Aqueous Solvent 

0.779 HNO, 
1.558 " 
3*75 " 
5.00 



(ina. t0. Par 
lOOcc one. sol. 

0.4421 

1*2377 

4-6670 

10.4160 



of Acid in 
Solution 



0.779 

LS58 
2.337 
3-75 
5*00 



0.0303 
0.3083 

0.75*7 
3*53^0 



LaLAHTHANUH 8<x> 

LANTHANUM CHLOB1DE I,a r,l,. 



Cl 



TY OF LANTH\Nl!M ClH.OHlDJ', ANI> OK LA NTH AM I'M O.XIDK IN AQUEOUS 

Soi.uTioNrt OF AMMONIUM ('*iu.oim>K AT 15, !U') U , 50 AND i(K) . 

i Pramlll uiul Uaurh.'iiht'rjji'r, WO,! 

The results are givim only in lh< form of small Houl< diagrams and it i s stated 
that the numerical data will b< publishi'd in I'ull in th^ dissertation of Johanna 
.KauchonborgtT, University of Mum-hen, io,vo. 'l'h<* equilibrium 

.ll ,-= LaOl-., i 'I Ml s *H 3 i! ,() 



was approached by 'the authors from both nidon. ^ Tin* composition of the- basic 
chlorides obtained by shaking th<* oxide with i.o n NH 4 ('I at dilTc-renl. lompo.ratures, 

and drying over soda limo, was approximately an follows : 

At i5, La 4 Cl 1 O a .9lIj|(); nt 'lo rt , L 3 til O 4 .0 li a U ; at :w<>, U H Cl, O^.i 
LAMTHAMOM Hexa Antipyrine Per CHLORATE CLat(XX: io l! u N f ) e 3(Cl0 4 ) 3 

loocc sat. solution of Laflthaisum ilex*& Aatipyriae Perchlorate in Vater 
contain 1.48 gm.CLa(01C 10 H ip N R } 6 3ta0 4 l s *i a , lWilke-Irfurt and 
Schliephake, 1928.) 



CrO 



ID 



LAMTHANUM 

100 gws. sat. solution of Lanthanum Chmmate in Water contain o.oao 
gm. ^<Cr 4 ) 3 at 35. tBritton, 1924 . ) 
LANTHANUM Potassium CHEOMATB. 

The system La t (O () 4 ) -K K s Clr C) 4 ! H t () at v/> wa HtuduMi by Carobbi, 1924, 
but Ibo' table of results ilot'H not hhow th< quantity of La t ((> O 4 ), present in the 
solutions. The renults xhow I hi" tirveritl tiuublt* i-oixipoutKiM formed. 
LANTHANUM Hexa Aniipyrinc IODIDE CL4l^C lo H Sp N f ) f ) I y 

loocc .sat. solution of Lanthanum liexa Antipyrinr lodidr in Water 



contain 29,50 gm. [ ' 

Schliephake 1928.) 



I at 



and 



IODATI La(IOi)i. 
SOLUBILITY IN WATER AND IN AQ. SALT SOLUTIONS AT 

lliifkift% ttftiS IVdftf, |t|ifV) 



25 



looo gms. H 2 G dissolve 0,6842 gin, LaCIOjh at 25*, dy nat. t 


k>l. 0.99825. 


Ccmc. of 


Cim*. | t i| 




t'unr. if 


(fflf I ^ 0f 


Salt, Salt, Milli- 




Salt. 


SU. MiUi- 






per Liter, &"> ^> 




Nurmftl. 


per Liter, St. Sol. 


La(NOt)s a ' 


0.5595 90732 


NaNC> 


95 


0.^901 


,00250 


S 


0,52$$ 0,99807 


14 


50 


o . 94^040 


,00385 


10 


0,5194 


II 


100 


i .. 1603 


00742 


So 


Q,$$23 


,00211 


II 


2OO 


i . ^85 


,0090 


100 


0,6214 


.O066t 


li 


400 


1.636 


,02422 


200,52 


0,7431 


,01533 


14 


800 


2 . I $6 


,04677 


KlOg 0.0990 


0,6290 


, 


4 


1600 


3.859 


.09005 


* 


0.4957 


0.5633 


,00037 


II 


JJOO' 


3,030 


,17243 


I 


0.9914 
1.9828 


0.4970 


,00030 
,00031 


^NiSScii 


1 16.34 


0,631 


,00112 


Na 


I0i 0.0913 


0.63538 


.00060 


I* 


5a.68 


0.674 


00355 




0,4560 


0,56466 


,00050 


li 


105.36 


0.754 


,00971 




0,9130 


0,50*835 


,00065 


u 


158.04 


0.816 


.01608 




1.8260 


o , 39938 


..00065 


It 




o 8117 


,02183 




3-6530 


0.19736 


,00069 


t* 


303-6? 


i . 063 


.04343 




4-5326 


o. 13393 


.00083 


4 


77 35 


i 3(14 


,08286 


6.7989 


0.09733 


,00130 


it 


1574 70 


1.^*3 


, 16652 



According to Rimbach and Skhubert (1909), one liter HjO tit** riven 1.681 gnw. 
Li(IOi)sat 25, determined chemically, ami 1.871 tfm, determliietl electrolytic-ally; 
solid phase, 2La(IO t )i.3HiO. 



891 



LANTHANUM I 



SOLUBILITY OF LANTHANUM IODATE IN WATER AND IN AQUEOUS 
SALT SOLUTIONS AT 25. 

(LaMer and Ooldwan, igj*); Friedman ami La Her, 19M.) 

The solubility of lanthanum iodate in water varied with different sam- 
ples from 0,00089 to 0.00094 g m - mols. per liter ( z 0.5907 to 0.6233 fns. 
La(I0 8 ) s per liter). 



Mola. salt per liter 


Mols. La flo g ) R per 


Mols. sa.lt pur liter 


Mols. La (10,,),, pr 


ol Aq. Solvent 


liter sat. solution 


of AQ. Solvent 


liter ant. solution 


0.0002 K ? S0 4 


0.0009167 


o . oo i KCl 


O.OOO91 13 


0.0005 " 


0.0009746 


0.005 " 


0. GOO 97 4 9 


o.ooxo " 


0.0010564 


0.010 " 


0.00 10 32 2 


0.0020 " 


0.0012153 


0.05 


. 00 1 H U 


0.0070 " 


0.0016852 


0.10 " 


0.001571 \ 


0.0125 " 


O.0020272 


0.10 " 


0,0016480 


0.02 " 


0.0023675 


O.20 " 


0.0018776 


0.05 " 


0.0031871 


0.50 " 


o. 002 56 a i 


0.05 " 


0.003370 


1.0027 " 


0.0030547 


o.io KNCL 
o.io NaNO, 


0.001679 
0.001654 


2.00 " 

0.05 Na ? S0 4 


0.0037828 
o. cnvn.tf) 


o.io NaCl* 


0.001627 


0.0333 LA ? (S0 4 ) ? 


0.0018 Jto 


0.033 kaCljj 


0.0009233 


0.0166 " 


0.0015 ^. 




Mols. aalt per littr 


Mols. Uafio,)^ ptr 






or AQ. Solvent/ 


lltr sat. solution 






0.00166 La(NO^)^ 


0.0008347 






0.00333 " 


O.OOo8iOi 






0.0166 


0.0008696 






0.0333 


O.O009V>8 






o. 050 Mg (NO ) _ 


O.001766 






0.05 MgCl,/ 


0.001768 






0.05 " 


O.O01739 






0*05 Mf?so. 


O.00301O 






0.05 " 


0,002997 






0.05 CdCl 


0,00l68t) 






0.05 CdS0 4 


0.00'UOS 





LANTHANUM MOLYBDATE 



One liter H p O dissolves 0.0179 gm. La^tMoO ) *it 
at 85. (Hitchcock, 1895. > 



o.ou** 



EQUILIBRIUM IN THE SYSTEM LANTHANUM HOLYHDATI, Sonm 

MOLYBDATE AHD WATER AT 2^. 



Solia 



Qua. per 100 oas. <AL. sol. 



0.77 0.01 La ? (Mo0 4 l^.aq.* i. la 15.50 

2.1414 0.02 1.1.2 16.19 

2,92 0.03 " 20,02 

7.56 0.08 " 22.35 

11.50 0.13 ." 25.26 

11.54 0.13 " 1.2.3 2S.27 

11.52 0.13 1.2.3 



too AS. mi. -."i. 



1.1.2 - 



1.2.3 



a LANTHANUM 



8Q2 



LANTHANUM NITRATES a and ^8 La(NO^ 



SOLHBILITY or LANTHANUM NITRATES IK WATER. 

(Fritna, 1935, ) 



tef. LKNOg), 
1 100 9s. S&t. 


yr Solid 

sol. Phase 



18.4 


50.03 
54.i6 


<x La(NO,) 5 . 6H,0 


21.2 


55-03 


" 


35*4 
42.4 
44*2 


59.12 

63-84 
65.13 





43.0 tr.pt. 
14.4 
15.2 


56.27 
56.94 


ft La(NO s ) s .6H*O s 



Ow. U(NO S ) S par Solid 
100 w, MU sol. Phase 



16.0 


56.74 


23.3 


S8.7 


29*6 


60.08 


32.2 


61.34 


40.0 


62,71 


46 . 4 


65.5S 


49.4 


65.17 


56.0 


68.30 


6S4 * 


1-pl- 75-04 



SOLUBILITY OF LANTBAHUM NITRATE IN AQUEOUS SOLUTIONS or NITIIC ACID. 

1037.) 



<u of 

aat. sol. 



1.771 



Results at ; 
(siuji. pr 100 mn. 

.u , V.JX , 



aoua 



1,489 
1.483 



1.929 
1.912 
1.892 
1.852 
1.880 

1.755 
1.645 



1.419 
1.440 



59. 


0.0 


56.42 


3.06 


46,42 


11*95 


29-10 


34.69 


29.63 


40, 17 


28.73 


41. lit 


25.18 


54-41 


21.61 


58.16 


3.79 


70*70 


0.56 


87.85 


0.0 


90*0 


Results at 


so" 


66.65 


0.0 


61.31 


a.59 


61.85 


. 5*39 


$6.70 


13.05 


56.34 


14*93 


44.21 


37.73 


30*31 


44*48 


39. $8 


50-51 


S.48 


78.31 


1*38 


85-S1 


0*41 


91.15 


0.0 


9G0 



UNO) 



.611,0 



3^0 



Hone 



U(NO 



''3* c 



Hone 



8 93 LANTHANUM 

LANTHANUM NITRATE La(NO 8 ) a . 
SOLUBILITY OF LANTHANUM NITRATE IN AQUEOUS SOLUTIONS OF LANTHANUM 

OXALATE AT 25 AND VlCE VERSA. (James and Whittcmorc, ion.) 
Gms. per TOO Gms. Sat Sol. Solid Phase Gms, r>cr 100 Gms. Sat. Sol. ^.^ 



La(NOj) 3 . ...... 

o 60.17 La(NOi)3 not det. not det. 

0.67 59-91 " 3.32 42.27 

2.10 59.03 " 2.80 38.50 

2-23 59 - 3 " +La 2 (CA)a.3H 2 2.51 35.57 

2.26 58 . 22 La^CaO^svjHjO 2.21 3 1 . 53 " 

2.34 55.20 " 2.01 28.63 " 

2-47 52.74 " *-46 22.15 

2,59 49-84 " i -18 17.99 

2.68 45.26 " 0.50 9.89 

not det, not det. LajCCA^sHaO 0.28 5 . 06 

SOLUBILITY OP LANTHANUM NITRATE IN AQUEOUS SOLUTIONS or MAGNESIUM 
NITRATE AND VICE VBRSA AT 20. 

fDl Capua, 19?9.) 

OBB. per 100 gps. sat. sol. Soliu Gtas, ptr 100 HP, sat. aol. 



60.13 o LalNO H ) 3 .6H^O 26.0 2^.0 U(NO I .< 

58.91 2.20 ' ' " 22.90 25.148 MglNO,)g.rt 

S5-o6 6.21 " 15.35 30.93 % " 

50.li 9.83 " 6,89 36.30 

42.98 17.40 " 3.20 39.25 

37.02 19.25 " o.o 43.68 " 

SOLUBILITY OF LANTHANUM NITRATE IN AQUEOUS SOLUTIONS OF MANGANRSE 
NITRATE AND Vic VERSA AT ao. 

(Hi Capua, 1929.) 



iihJISi: 8olld <* p r l a - u w>x. soiia 



6o<1 3 o.o La(N0 3 ) 3 .6H 2 34.70 26.80 MnlNO )^.6H 

53-90 5.08 w 22.95 37.50 " f 

49.20 8.91 " ar.as 39/18 

41.45 13-22 " 14,13 <u.j 

36.82 16.19 " 10.00 4S-00 " 

29.8l 21.00 " 6.22 49.20 H 

27.45 21.95 " 0.0 58.81 

LANTHANUM Magnesium NITRATE aLalNO^^MgtNOg^.ai^O. 
SOLUBILITY or LANTHANUM MAONISIUM NITRATS IN WATER. 

ffrltnd aria Whau 1955.) 



pr 100 rfjna. aat, aolutlon c per 100 Hn- 

l8 * 6 62.19 61.4 7305 

3]-6 63-96 74.8 77.43 

46t8 68,57 U3.s(m.pt.) 100.00 
50.8 70.17 



La LANTHANUM 894 

LANTHANUM Ammonium NITRATE La(NOi)a.2NH 4 NOa. 

joo gms. HaO dissolve 1814 gms. La(NO 3 )j.2NU 4 NOj at 15- (Holmbwg, I907 .) 
LANTHANUM Double NITRATES. 
SOLUBILITY OF LANTHANUM DOUBLE NITRATES IN CONC. HNOa(<fu = i. 32 c) 

AT 1 6. (Jantseh, xyu.) 

,. . tJnis. Hydratcd Salt 

Salt. I'ormuhi. 1 hssolyed per 

Lanthanum Magnesium Nitrate (La(NOi))*Mgi.a4Hi() ' 63 .3 

Nickel " \ k * \ t 80.3 

" Cobalt " t | >-a u *QQ.2 

" ^ inc u M l " 4tl 

" Manganese " * Mn^ 193.1 

loocc. of a saturated solution of UlNU^^Fy) in Ethyl Ether prepared 
by freiuent agitation and allowing to si ami* over aight at about 20 con- 
tain 0.002 gm. La . A saturated ethereal solution prepared as above 
but using Lanthanum' nitrate dehydrated at 150* contain only o.ooi gtn. 
La^O per loocc. (Wells, 1930.) 

Fusion-point data for mixtures of LatNO.,1,, * Mg(NO n ) f Are given by 
Quill and Hobey, "- 



by 
NO 



LANTHANUM OXIDE La^. 

OF LANTHAHMM OXIDI IN WATIR. 



n m ^ ^ 

c ptr liter sti. aol. , , . . , . 

jLg 0.405 Poteniicxnetric Suiolxn, 1937.) 

2S o.uo* Volumetric Bush, i*>a7. 

25 0.73 Volumetric Kolthoff *md Rlmquist, 

25 0.3-0.67 Cbndiictivity tf 1931. 

LANTHANUM Dimethyl PHOSPHATE Ut[(CHi)flPO 4 I.4HiO. 
100 gms. H0 dtBiiolvc* roj.j gnw. Las((C.'!!a)j|! > ()4{t^t 25**- (Mwr*nnil 



LANTHANUM SULFATE 

SOLUBILITY IN WATKK. (Muthmann ami i<% t i 



r 

* 



Solution. Wittrr. * Nluiwm. Waittr, 

o 2.91 3 50 1,47 *.$, 

14 2,53 a, 6 7S o,Q5 0,96 

30 1.86 i.g too o.f>8 o,6Q 

SOLUBILITY OF LANTHANUM SPLI-ATK IN An>. NtHj'iioNs 01- AMMONIUM 
SULPATE, POTASSIUM SIILFATE ANI S<mt'M SttJ'\rf. titarrf, io, 1911.) 

In Aq. (NHOiSOi at 18*. In A<|. KiSO 4 at ic 5 J , In A|. N.nS() at i . 

(Jms. per 100 Gms, H^C). Stlui I'l^Li^J^Lf!. 1 !!!-'^* W**l <*m-. Kt i^fcttiin^HiO. Solid 

Phase. 




4.OI 0,393 I - 1 ' 2 

8.73 0.279 

18.24 0,253 ** 

27.89 0.476* " 

36,11 0.277* " 

47.49 0.137 2,5 

53.82 0,067 1,5 

6S.2Q O.OII7 " 

73.78 0,0033 u 

* * iit*tlr r|iitfiltfi{fit 

i.o.o l^as(S04)i.9HiO f LI.J I*fii(SC^H VjS() 4 ,/Hj(> (wln*rt .V - a (NHi)* 
K or Na), 2.5 - 3Ui(S0 4 )i.s(NHi)SO4, i.s Iij f SO 4 ),..v\'|Si> 4 . 



895 



LANTHANUM 



SOLUBILITY OF LANTHANUM SULFATE IN AQUEOUS SOLUTIONS OF SULFURIC 

ACID AT 25. (Wirth, 19x2.) 



Normality Cms. per 100 Cms 
of Aa. bat -, boL 


' SS " y Gms '^^ Gms * 


Solid 
Phase. 


H2S04- LasOj 3 * LaaCSOJs 


H 2 SO<. JUjOa * I*a ? ($O 4 )n. 




Water 1.43 


2 


.483 


Laa(S04) 3 .9H 2 O 4 , 


.321 


i. 


.11 


I 


.927 La 3 (< 


SO^a-gHjO 


o. 


S5 


1.69 


2 


934 


6, 


685 


0. 


531 





.9217 


" 


i , 


.10 


1.796 


3 


.118 


9 


.68 


o. 


,266 


o 


.4617 





2 . 


,16 


1.818 


3 


.156 


" 12. 


,60 


o. 


214 


o 


371 





3- 


39 


1.42 


2 


465 


15. 


15 


o. 


177 


o 


307 


" 


Data 


for the solubility 


of lanthanum sulfate in 


aq. 


HaSOi in presence 


of solid 



oxalic acid at 25 are given by Wirth, 1908. 



LANTHANUM Ammonium SULFATES. 

EQUILIBRIUM IN THE SYSTEM LANTHANUM SULFATE, AMMONIUM SULFATE 

AND WATER AT $5. ( Zamlxmini and Stolfi, 1M6.) 
(",ms. per 100 gins, snl.nol. 



0.88 

0.88 

0.75 
0.73 

o,3o 

. 9.8 
0.0:6 



6.^4 



1 1 . 1 1 

9,2.89 

9. a . 80 
9,5. 19. 

^7-97 



Solid P)ia. 



ilUN. JKM- 100 glllS. ftt. SOt. 


r.a a (so'l),. " 


(Nll,),80 4 . 


O.22 


9,9.37 


O . H) 


3o.4o 


O , O r ) 


33. <> 


O . O.5 


30.8"> 


O . O'l 


39.9,4 


. 02 


4a.4 


O . Ott 


43 . a4 


O . Of) 


44,64 



Si 



. 
= La 2 (S0 4 ) 3 .3(NH 4 ) 2 S0 4 ; 



i.5La,(SO 4 )a.5(NlU)aS0 4 ; 
i.f, La t (SO 4 ) 3 .6(NH 4 )tSO 4 . 



LANTHANUM Potassium SULFATBS. 

EQUILIBRIUM IN THE SYSTEM LANTHANUM SULFATE, POTASSIUM SULFATK 
AND WATEK AT 45. (Zumbonini and GarobM, i>4.) 

Gins, per loo gins. snl. sol. 



U,(S0 4 ),. 


K a SO,. 


Solid Phnv, 


0.87 


o.a3 


t . I 


9, 


0.77 


0.9,3 


)) 




0.41 


0.45 


> 




0.9.8 


0.79 


2.3, 


,8 


. 9.6 


0.74 





-4- 


o . 9.4 


0.87 


i .: 


1 


o.oo 


1. 62 





-4- 




1.5. a 



1.4.1 



La LANTHANUM 

LANTHANUM Sodium SULFATB. 

EQUILIBRIUM IN TMK SYSTEM LANTHANUM SULFATB, SODIUM SULFATE 

AND WATER AT 4f5. ( Zaailnwmt and Oawbbi, lM>a, | 

Cms per lOGfliiiK. snl. sol. imv per too gins, int. ol< 

i^^-.-^J-^l. Solid *-..- .^ Solid 

La a (SOOs. Na s SO,. 1'hase, I.,|SO,ii, NA,SO,. Phwe. 

O.KJ 0.5.J U,,uS0J a ,NiitSO,,'!lM> o.(^ 10.40 tailHQtii.NiitSOt .111,0 

0.09 0.75 - 1 3. HO 



SeO 



trace 



7.1:* 



$ 8 , 06 



* Xa, SO, 



LANTHANUM Thallium SULFATES. 

EQUILIBRIUM i 

A^ 

GUIS, pci* 100 gins. Mil, ,soL 



HQUIMBKIUM IN THF. SYSTKM LANTHANUM SULI-'ATK, THALUUM SULFATE 
AND WATER AT 25. { Zumlmnim tttut C,aruhiti % IM5, ) 



Solid 



i.8.{ 0.19 

i , 1 9 o . 1 4 

0.29 <>.49 

0.19 0.84 
o . 1 5 



i .% 
u.ot 



i'/i 



O.^7 
0.25 



.27 

.75 

.71 

,82 



4.07 



i .3 r-= !- 

,. | */ s TLS 

SOLUBILITY o? LAHTBAHWW SILBKATI IK WATER, 



+ TI,S0 4 
)i.3TI,S0 4 ; 



0.0 

9.6 

15.0 

21.8 

25.4 
33.6 
40.6 
36.4 



100 4P. ftt* Ml. 

33.55 
30.90 



30-54 
31.89 



Solid 

FhMt 



69*4 
78.2 

81. a 



34-00* 



37-54 

ai-17 



5-03 
I.7H 

1.97 



* Meta3table 



SOLUBILITY or IAWTHAMUM SILENATI in Aatiiotts SOUITXOHS or SILINXC ACID. 



(>>a pr 100 jaa. 



80iia 



35 



o 31.3 

2. 08 a8.^6 

7*80 24.07 



. s A ^ ^* 



LANTHANUM TUMOSTATE 



One liter HLO dissolves 0,0117 
(Hitchcock, 1895 J 



^}. AI a? f d 0,0.316 ai 65 



&97 LITHIUM ; 

LITHIUM Li 

SOLUBILITY OF LITHIUM IN LIQUID AMMOHIA, DETERMINED 
BY VAPOR PRESSURE MEASUREMENTS. 

(Joimaon & Plalcur, 1933.) 

The vapor pressures of solutions of lithium in liquid ammonia at 
constant temperature give a curve which intersects the horizontal Line 
representing the vapor pressure of the saturated solution. This point 
was determined at several temperatures with results showing that, con- 
trary to the determinations of Ruff and Geisel, 1906, a slight increase 
in concentration of lithium in liquid ammonia occurs with increasing 
temperature. 

Vapor Prtssur Mola. NH^ ptr Q*s. LI pr 

1 a. Hrf. atom LI 100 P. KH^ 

-63.5 1.1 3*8l 10.698 

-33.2 3^ 37S 10.866 

-32.7 3.4 3-7U 10.89$ 

o.o 34-0 3-60 11.319 

LITHIUM ALUHINATE LiH( AlO^) ? . sH ? 0. 

One liter sat. solution of LiH( AlO g ) g .sK ? in Water contains 0,00012 
gm. equivalents at 25 0.00013 at $0 and 0.0003*) at 80 as deter- 
mined by electrical conductivity. (Prociv, 1929.) 

A 
IJTHIUM AKSBNITE LiAs.Oj. 

EQUILIBRIUM IN THE SYSTEM LITHIUM OXIDE, AH^KNH; THIOXIDB ANW WATKH 

AT ^5. (Schroiuiink(iri!i arid di Bt, li^O.I 

Four to six weeks constant agitation wore required for natur&ttoti, 

r ' mMt t>r 10 m * nnL H0ti 




LiAsOt 7.3") 7.47 

7.64 ;.5o 

7.81 3.8i 

4.24 5.65 ? .i> o.o 



LITHIUM BORATE (Meta) liB0^.8H 0. 



WO M MC. Ml. 



SOI.0BII.ITT OF LlTHIOK MlTA BORAT1 IN WATMU 
(Rooenheia a/id Rglin, igm Mmml, ton.) 

par Solid o*s. UBO ptr doll* 



100 pM. Mt. Ml. 



-0.515 0.78 Ice * UBO .8H f O 25.6 3.0 LiBO^ 8HJ) 

- - 8 ^ LiBO^.sB^O 38,8 9.42 1 f 

18.0 2.203 '" i| 4 .8 ln.7 w 

3 5o 3-344 " ^7, m.pt. 



Li LITHIUM 

EQUILIBRIUM IN THE SYSTEM 



Gms.perioo,Gms.Sat.SoL 



BO 



Li 2 0. 


BA- 


y.OI 

7-51 
7.71 


2.98 
3-3B 


7.68 


? , "5& 


5-40 


2 , 78 


3-47 


2.42 


2.94 


2.51 


1,58 


3-27 


2.17 


6.90 


3.66 


14.78 


5-25 


22 




23,8 


i'.8i 


6.20 



] phaMr 



OXIDE, BORIC OXIDE, WATER AT 30, 
1, 1907.) 

100 Hrm, Sit Sol, 

* Solid Phase. 



LiOH.H/) 



o*,86 


2.47 


0-53 


2.4? 


2,17 


IJ, 12 


2,61 


l6,3<) 


S o8 


30, Si 


4,10 


27,07 


3,22 


15,40 


i, ss 


IS.40 


1,3.0 


14,14 


o.<)6 


11,47 


0,63 


4-% 


o 


3-54 



J_ t Q JL V **' ~ -'--- 

LITHIUM Per BORATB 11,8,0^.3*11,0. 

100 cc water dissolve ,0.13 Hi""" P* r bt>r * te " ordinary tefflpera - 

ture. (Bezaer-Ldwjr, 19^3* J 

Fusion-point data are give* for: 



UP (Kitadgorodski, Popow* *a<l Boiwinkln, 
Li SiO, (Klooter 1910-1 iJ 
S 



UBO 



LITHHJM BEOMIBI 



SOLUBILITY IN WATBR. 

^ 1858; 



Br 



feft Cms, UBr DJT M ^ pj,^. 
fc ic Gros. HiD. 
- 0,46 1.058 toU) 
- 1.94 4.274 Jl 


l tm*: t UBr |*ei 

10 166 

20 I?7 


' Snlk) WUUMB. 


- 4.27 8.678 


30 10 1 


44 


-10.3 17.80 


40 2O5 




30*5 37.64 ** 


44 300 


** fUBr.HiO (B) 


AC <o ** -fLIBr.iHjD 

s 

30 oO OBr.sRW 


So 214 

60 334 


UBr, IliO (K) 

ii 


IO 122 ** 


to 34$ 


H 


o 143 ** (K) 


100 266 


4* 


+ 4 160 ftlBr s fH^CD 


ISO 


Uf.H/HUBr(B) 


The more recent dettrmlauioa* of lltt: 


tig ami Rf?tctiif t?*** wd of 


Httttig aad Steudewanft! 1927* ^y *^ fr^itft|-poifti mnitipai > 
not agree with the above older reuii espeeUlly for ihe ill *w in 
hydrate. The following values wtrt takea Iron cur* con- 
structed frow the result* of Httitif d co-orkr. 


(toa. L10r pr loll 4 


aw. Lltr *r fcUJ 


1 100 a. i*t. Ml. f'Hase 


* too P^. ^- 


Mi. IM4 


-72 39 a Ice * LlBr.sM) 

-S3 47,9 LiBr*sH f O * lfr.3H f O 


35 ^1.0 

|2 65. t? 


1 UB '?iBr. 


-30 51 o LiBr*3Hj|0 
-10 S5*o " 


31 67-61? 
40 67.8 


1 


* 4 59,2 *LiBr.aH r O 


60 60*0 


H 


10 S9*S LiBr.^ F 


80 71.0 


If 


20 61.6 * 


100 73.7 





8 " LITHIUM I 

SOLUBILITY OF LITHIUM BROMIDE IN AQUBOUS SOLUTIONS 
OF HYDROBROMIC ACID AT 25. 

(Scott and Durham, 1930.) 

Qns. par 100 gna^ sat. solution Solid 

/ HBr LiBr ~~^ Phaae 

o.o 60.41 LiBr.aHpO 

5.44 55-29 " 

23-93 38.09 H 

29.90 34-45 " 

SOLUBILITY OF LITHIUM BROMIDE IN AQUBOUS SOLUTIONS or 
ETHYL ALCOHOL AT 25. 

(Slnaona. Fr el much and Rusaell. 1936.) 



(tea. per 100 


ipa. aat. aol. 


Solid ana. per 100 


B.isa.t.^sol. 


Solid 




' W H 


LiBr s 


Phaaa ' <yi g OH 


LiBr 


Fhaao 




0.0 


65.31 


LiBr.aHgO 43.28 


47.63 


LiBr.H. 





4.88 


62.08 


" 47.57 


46.70 


M 




10.23 


59.06 


" 46.53 


46.63 


" 4> L 




14*44 


56.68 


47-86 


46.. 51 


LiBr 




20.09 


55-24 


51.66 


44.13 


n 




26.59 


52.98 


11 55-24 


42.45 







33.05 


52.07 


11 + LiBr.H g O 58.78 


41.22 


ti 




35.43 


50.79 


LiBrHj,0 









SOLUBILITY OF LITHIUM BROMIDE IN ABSOLUTE KTIIYL ALCOHOL, 
( Honnoll and Jones, ll)ii(i. ) 

* nr M/O rms L r n n orr IM!'!!! Between *3.a anda,V.8 lithium bruinidc ulco- 

t . po. 100 gm, ,i. t ii, oir. h.. 



...... j'l.oi LilJr depending upon the solid phase 

10 ...... 36. 0^ Gmg. U Dr pr oo mi, 0, ll fc (>ll 

7,5 ...... 7*2. TO jjrhjntho Solid Phn IN 

3o ...... j'l . 5 1 t M . n iir. 1.1 r.4 c: f n. on , 

4o ...... 78.03 i 'J . v. ...... 70 . o 70 . o 

DO...... 77.57. if, ......... 70. v, :j8.i (58.7) 

60 ...... . 82.84 16 ......... 70.4 '19.0(67.5) 

7<> ...... 89.13 uo ......... 70.8 /fc.o (fto.tij 

75 ...... 9i- ia )} a3... ...... 71. ,* 46.0 (S3. o) 

80 ...... 99,10 a3.8 ....... 71.3 47.% 

The results in parentheses were obtained by thermal analysis. Thn outoctio 
point for Li Bi + Li Br.4 C 2 H 5 OH is at i3.a. The congruont m. pt. of 
LrBr.4C,OH is a3<>.8. F 

SOLUBILITY OF LITHIUM BROMIDE IN AUSOUJTI ACITOKB. 

(Bell, Rowland^ Bfuaford. Thoau and Jouoo, 1090.) 

(tea. Li Br per Solid o as. Lt Br par 

L 100 a. (CH)^CO Phaa 6 100 DBS. ^ CH ) CO 



jCO 35.5 22.6 UBr.a(CH ) 00 

20 18.2 " 37 a37 UBr 

30 21.3 " 40 26.3 " 

32 22.1 " 50 34.6 " 

35 22.4 " 60 39.7 " 

Determinations made by means of specific conductivity meAsurements by 
Lannung, 1932, gave 11.24 gms. LiBr per 100 gms. (CH^).CO at i8 8 and 
19.8 gms. at 37. * 

100 gms. Glycol dissolve 60.0 gms. LiBr at 14.7. (deConnick, 



Li LITHIUM 900 

LITHIUM BROMIDE 

100 gws. sat, solution of lithium bromide ia Bens&ldehyde (C.H 010) 
contain 11.527 gms. LiBr at 25. (Miiller, Raschka and Wi ttnann, 5 i 927 .) 

Fusion-point data are gives for: 
LiBr * UC1 (Botschmar, 



UC1 
LiF 

LiOR (Scarpa, 1915*! 

AgBr (Sandonn ini aad Scmrpa, 

KBr (Kellner, 1917* * 

MgBr (Keliaer, 1917; Ferrari and Call a, 1931. 

NaBr (Kellaer, 1917. * 
(Kellner, 



BrO 



CH 



LITHIUM BROMATB 



100 ( 



5 

IS 
25 

3S 



63.3 
6$, 4 

67.5 
71.5 



OF LlTIXflH BtOMATI IK WATIt. 

Jft we* wtioMk, i93t.) 



53 
56 



Solid 



73. 

73.6 



LiBlO 



100 



70.0 



is between 



The transition tetiper&twre for iiBi0 3 .H f O 

So. 8 and 32. t it* 

The previous determination of Hylius aa<i Punk, i^gy tfk &f 6o*<* gms. 
LiBrOL per 100 gms. sat. solution of density - 1.833, Is appArantly too 
low. 
LITHIUM METRIOMATE Li f lCT f (SO^ )^J, 

100 gins. H f O sat, with lithium Methioaate cofttain 7a t 8 

Li^CCH^OO^Jjg] at as . (Baker and Terptr*, 1939; Baker, 1930.) 

LITHIUM FORMATE LiHO)D.H f O. 

SOtOBXLXTY Of LlTKXtm POt*ATI XN VATIft. 



r. 

20 



18 

49-5 



Gnw. 

HCOOLi MCOUW &.MA nij.^ 

per 100 Gmi, pr 100 Mk. mm l mm * 
Solution. H|0, 

21.14 9.28 HCOOLlHjO gt 

24,42 11.18 " gH 

27-8$ 13.36 4i 104 

ig,t4 " i jo 



tm*. M(d. 

^wn^ 



S4.t6 

57 05 
57 ( *4 



40 cx> 
45 W 

47 , l ! 



!!C:(K)Li,HiO 
I!CCK)Li 



74 44,91 28,21 ** 

Sp, gr. sat. aol. at ,J8 1.142. 

FRERZINO-POINTII OF AQUKOUH LITIIHIM FORM ATI-: SOLUTIONS, 



ami Uc 



901 LITHIUM I 

FREEZING-POINTS op MIITURBS OF LITHIUM FOKMATI AHD FORMIC ACID. 

(Kendall and Adi or, io?l.) 

The previous results on this system by Groschuff, 1903 are considered 
to be largely in error. 

(ta. Mols. L1HCOO Solid Q. Mola. UHCOO Solid fl Qfe. Mols. LiHCOO Solid 
1 per too * nola. Phft* per 100 pi. w>la. Phaa c per 100 ga. MO!. Phase 

all cure sail cure lxcur 

LiHCOO 



8.4 


0. 





HCOOR-14 


.6 


18. 


19 


ncoon 


90. 


5 


25.91 


7.0 


1. 


58 


?t 


-17 


.1 


19. 


56 


it 


97- 


9 


26.38 


5.2 


3 


47 


ti 


-19 


.8 


21. 


05 


rt 


113- 


1 


27.71 


3.2 


5* 


23 


M 


-21 


7 


22. 


24 


" 


131. 


2 


29.87 


1.1 


7. 


09 


ft 


-23 


5 


23- 


49 


l 


14S 


1 


31.98 


-1-3 


8. 


93 


H 


-25 


.0 


24. 


33 


rt 


ISO. 


4 


33-04 


-3.5 


10. 


75 


If 


n8 


.0 


23 


49 


LiHOQO 


159- 


1 


35-01 


-5.6 


12. 


23 


II 


34 


.0 


23. 


98 


tv 


163. 


5 


36.13 


-8.2 


13- 


99 


It 


80 


.0 


25 


31 


t 









LITHIUM ACETATE CH 3 COOLi.2H 8 0. 

SOLUBILITY OK LXTUIUM AOKTATH IN WATJKH. 

uiul (xuiillc, 10*22.) 



<>ms. CH;, CO 

t"- per KK gnus, si 


on solid 

ll 80 1. 1* lilt SO, 

Ice 

GH 3 GOOLi.ttH,0 





<.nts. Clf^'.OO l.l 
t s . IXM* urn gniK, Nat. Mil, 

53.3 . "i-i .7 rti 


1 6 . i >, . . . 


4.83 
. 9.53 
. 18.33 


-)5.4 


6 (.?/*> 
(>4.88 
() 73. 




r >7 . Him*, pl.i. 


2~) 8 


3i ?8 


lo?,. 8 

1^7 r * 


36.7 


. 38. a5 









FRIIZING-POINTS or MIXTDRIS or LITHIUM ACITATI AW ACITIC ACXP. 

(Davldaoti and He All later, 19^,) 



c L1C 2 H 32 p * r 8oUa *- <>^ WC ,V* ^ r oU CH 

100 an. OU. Hixuire Ph& l loo ^. W0U . Sliwrt PM 

16 -50 o.o H C 8 H 3 110.0 41.84* ui 

^ 8 S 3-56 M na.o 45.74* 

1(f ' 16 S.oi " ua.s 48.76* w 

1 3i5 6.86 " 112.5 50.06* M 

l ?' 10 8>lf5 " J 36.o 43.95 LiC.ILO. 

l6 * 7 8 - 61 ! 147.5 46.04 M 

2 2 - 1 9.15 " 156*0 47,57 

35 ' 9.53 " 161.0 48.22 

5i.o 12.28 " 178,5 53, m H 

2' l6 * 2 ^ H 8.o 55.89 

83 ' 20.25 M 192.0 56,90 " 

9 8 ' 27.64 rl 221.0 70,8? H 

Io6 '5 35-34 H 272. 100.00 
109.0 39.83 fl 

* Metastable; n = UC^H0,.HC,H,0.. 

* o K y, 5 g 

Preriou3 detenninations upon this this system ar given by Vnsilev. 
100 ems. methyl alcohol (CH a OHl sat. with dehydrated lithium acetate 

82EyS7' UCA at 15 aad 3X47 gms - al 67 - a (b - pt - 1 



Li LITHIUM 

LITHIUM Phenyl ACETATE 

Fusion-point data for mixtures of Lithium phenyi acetate (LiC H 00 ) 
and Phenyl acetic acid tHC-XCOj md * or Lithium pheayl acetate and* 
Phenyl acetic anhydride, (C 7 H 7 CO ) g Q, are given by Bakuain aad Vitale, 
1935. 



LITHIIJM CITRATE C,H 4 (QH)(COOLi),.4H,0. 

100 gms. IljO dissolve 61,2 gms. Li citrate at 15**, 



sat. sol. 1.187. 
(Grctnith and Smith, 1902.) 



CH 



SouraiuTY IN AQUROUS ALCOHOL AT 25. 

(SculcH, 1910,) 



cX'otf 


rf-ttOf < 


Cm*. 


Wt. *"i 


dtt t>f ( 


Cms, 
VW)H((XX 


insolvent. 


Sat, Sol. i 


|H|O mt 100 Gmti, 


In Solvent. 


Silt. Sol, j 







1.216 


74.50 


SO 


0.033 


4.Q3 


TO 


1.150 


4Q.30 


60 


o , 8i>7 


2 " 2 S 


2o 


1.083 


32,10 


70 


0,867 


0,60 


30 


1.025 


18.80 




o.H^H 


0,30 


40 


0.976 


9 ^5 


IOO 


0.788 


O.O2 



LITHIUM TARTRATES. 



SOLUBILITY IN WATKK. 



Salt Formula, 

Lithium Dihydroxytartrate 
Lithium Sodium Racemic Tarlrate 
41 " Dextro 

" Potassium Racemic " UKC 4 HA.IW> 

" Dextn 
THI SYSTEM LITHIUM AMMONIUM <f- 

ANl) 



Cm, Salt 
4*. f?r too Urn*. Authority. 

Sat. Sol. 

O 0.07Q (Knton, 189$.) 
20 19.97 (vhltwutjcrg, 1900.) 
20 22.55 *' 

m 37, H,* 
liTitm 



The saturated solutions aad the solid phwes ^ere ii,iyj(<t jmUri- 
metrically usiag as a acale the rotations of sotutiofta of pure Lithium 
Ammonium d Tartrate of different concentrations, tleicnniu*<i (or the 
sodium D liae at 30. The isotherm AI o wy det^miu&i and the 
invariant points only at 30 &nrt 60. 



30 



Qu. ptr 

'4 446 

0.0 
12*241 
23.251 

28*519 
0.0 



'X,, 



2.361 
1. 860 

1.64 

1 * 462 
0.98 



6.542 



RaceAte form C = 



** * d C0rm 
d forw 

H 

Racewaie forw 



903 
SOLUBILITY OF LITHIUM CI-TARTRATB IK WATKR. 

(Campbell and Slotin, iorw.) 



LITHIUM ] 



ans. LI 2 C 4 4 O e 
* per 100 gms. HpC 


Solid 
) Phase 




o . 42.106 


Li 2 C 4 H 0' 


-2H ? 


8.0 33*451 






10.55 31-495 
20.0 27.052 


If 




2i.67tr.pt. 


"+] 


^ C 4 H - 



25 

30 
45 

60 



per 100 aa. H^O 

26.711 
26.663 
27.510 
29.532 



Solid 
Phaoc 



EQUILIBRIUM IN THB SYSTIM LITHIUM CJ[-TARTRATE, AMMONIUM 
d-TARTRATB AND WATBR. 

(CaapDell and Slotln, 1933.) 



per 100 



Results at o 



Solid 

Phase 



Ons. per 100 g. )!,,() 



Results at 30 (con. ) 



0.0 


42. 106 


Li g C 4 H 4 O a .2H ? 


2.510 


36.857 


" 


3-473 


32.561 


" 


6.013 


30. 160 


"+ DS 


8.022 


22. 125 


DS 


14* 491 


14.092 


" 


23.08l 


8.846 


11 


36.6lO 


7.011 


" 


45*930 


6.026 


4 ? * 


45.125 


3.952 


(NH I,C 4 4 6. 


44.251 


1.973 




43-916 


0.0 


M 



24. 


662 


14- 


732 


DS 






29. 


651 


11. 


603 


" 






39. 


671 


8. 


182 


M 






63- 


600 


6. 


916 


11 






66. 


205 


6, 


771 


it 


*<NHA 


,c. 


66. 


310 


3. 


326 


<Nff 4 ),C 4 l 


V 


63. 


813 


0. 





n 







:jrOResults at 60 

H H Q 



Results at 30 



o.o 

3.076 

7.703 

9.350 

11.980 

14.672 

16.744 



26.661 
27.143 
29.181 
30.661 
32.731 
26.071 
22.603 



DS 



DS 



0.0 


39$$3 


5.807 


30.051 


11.003 


31 . 453 


16.349 


34.343 


23.121 


37.981 


24.43* 


27.609 


41.083 


l6. 151 


63*OU 


33.103 


98.39^ 


10.244 


92.832 


6.650 


90.347 


3.631 


87.171 


0.0 



DS 



DS 



'*(NH 4 LC 



m 



4 fl 



DS = WC 4 H 4 O a .(NH 4 l t C 4 H 4 O fl . 
LITHIUM BENZOATB <; H^COO Li J| t o. 

SOLUBILITY OF LiTirrtiM BKNZOATK IN WATKK, 

( Sidgwi<*k ami Ewhank, IOM. 
Cms. C H n,i(;OOLI 
t"- pt'r 100 gms. mi. sol. 

I . 69 .... 7 . '29. 



Solid 
IMut<*. 

Ice 



o./i()..., !<).:> ) m.o.... S<> 

2 ^7-97 QH 8 COOLi.Hj() Kiv.. /,.... 45.1,, 

" h '5-; ) ^- 8o 176.0.,.. /<i.iv 

28.5 3?.. 12 

100 gms. Methyl Alcohol (CH 3 OH) saturated with dehydrated lithium 

benzoate contain 20.52 gms. LiC H COO at 15 aad 19.71 gms. at 67 
(b.pt.). (Henstock, 1934.) 



Li LITHIUM 904 

LITHIUM BENZOATS QHiCOOLL 

SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 2s. 

(Seidell, 1910.) u 

Per cent j af Gms. CH s COOLi Per cent . . Cms, CHLCOOri 

C^fOHin -. p^-G*, Cg* *-. *** 

o 1.103 27.64 60 0.970 19.80 

10 i. 088 28.60 70 0.932 15^40 

20 1.072 28.50 Bo 0.890 10.70 

30 *-5 2 27.80 90 0.847 6^40 

40 1.030 a6,2o 95 0,823 4.^0 

50 1.003 23.60 ioo 0,799 2.60 

100 gms. HjO dissolve about 40 gms, QHiCOOLi at the b. pt. (U.S p) 

ioo gms. alcohol dissolve about 10 gms. CiHiCOOLi at the b. pt. " 

LITHIUM o Hvdroxy BENZOATE (Lithium Salicylale) (l c lU.OH.COOLi.U,0. 

SOLUBILITY OF LITHIUM ORTHO HYDROXYBKNZOATK IN WATER. 
, iiU fiwhmtk, 1M2, } 

<Jm. 

H;,JI, on. coo LI 
t firr iwxmi. nt K|. Solid Phono. 

u8 .*.., f 6 . 5o r> c.ii t .oir.coou.ir 1 o 
'J8.5.!! 5y.67 !! 

ro.*i... 66,56 ,, 

7 *4 ffft 1 " 

rH 3.5.... 5a.yC "'^"'""^'nlffl" n : !o!.'.' 71'.' <V " '" " _ ' OOL1 

*"'^ /v ^v <k *ifi .^Jfl fill i>/\i\ t t t /*. . *>O . w f ^j 

SOLUBILITY OF LITHIUM META AND PARA HY&itoxYitt-;N7.(>ATttM IN WATKIU 

Results * * Ht'suitf 

for Mela IIydroxybeny,oaie. for Psir* Hydrnxyhenzoate. 

Ontn. (iuiH 

mcn 4 ,o.t;ooi,i >iiii /<^II,.OIM:OOI.I solid 

t. per too m. *l. M|. IMww, t w JMT I MO sms, | <nl. rhuhf, 

* 4-4'.-- lo.oa Iri* 0.98,.. T i.t>4 Ice 

-10.78... at). 58 'i.'i;.., y.8i / 

- 17.67... 39.97 ">.'*'i... 17. HH M 

P.V "> o4 i "" r *t " ** ^ 

104.0.... 58. ,,7 * tu,' 3o.H{ /(;,.( 

12^.0 61.86 s : o. . ... 3o,tia i 





GIUK. 






o cn,.OH.cooi.i 




t". 


per iiKUius, snt. sol, 


Solid IMi^i' 


2.26 


... 10.17 


Ice 


5.56 


... W).6'A 





rI2.8u 


... 35.83 





8.5. 


... 45.20 <:j 


ir^.oH.tiooij.c.n/) 


1.0. 


... 49,0/1 





H- 9.0. 


52 , 4 5 <* i* & J 


n t ,oit,t:oou .,(> 


3.5. 


... 5a.t)(i "^ 


ri t .oi!.(:oou.nii.o 

ltirititiMHt*i 


10.0. 


... 59,96 <:,i 


[i t .(Mr.<;ooi.t.H M o 



LITHIUM S^ICYLATE CiHiOHCOOLLJUA 

SOLUBILITY IN AQUEOUS ALCOHOL SOLUTIONS AT 25, 

(SeWeJI, 1909, if to,) 



Cms. 
C 8 H & OH per 


* of Cl 


K<OHCOOH IH 


t\H C .OH *r 


rf f 


c Cms. 


zoo Grns. 
Solvent 


Stf. Sol, * 


per ioo Om*, 
Si. Sol. 


ioo Cms. S 
Solvrnt. 


tt! si. * 


per 100 Gm, 
Sftl.Sol. 


O 


I.2O9 


S^ 


60 


. 104 




10 


1,195 


S5'9 


7O 


.083 


4Q-S 


20 


I.lSo 


SS-4 


80 


.056 


47-5 


30 


1.163 


54-7 


90 


,026 


4S- 


40 


1.144 


53-7 


92-3 


,020 


45.6 


50 


1.124 


52.5 


IOO 


.027 


48,2 



ioo gms. propyl alcohol dissolve 18.7 gms. LI aalicylutc (temp.?). (Kchlamp. i 



905 



LITHIUM HIPFURATE C 6 H 5 CO.NHCH 2 COOLL 

100 ems. HoO dissolve about 40 gms. of the salt at 15-20. 

b ' " T-nun u r\ (Squire and Camus, 

LITHIUM PHTHALATE 2Ll 2 C 8 4 4 3H ? U - 

EQUILIBRIUM IN THK SYSTEM LITHIUM PHTHALATE, PHTHALIC 
ACID AND WATKB. 

( Smith, Stum ana Ely, 1935.) 



LITHIUM LJ 



Ctea. per 100 



Solid 



Otos. per 100j. sat - so1 * 



Solid 



Results at o" 



Results at 25 (con. ) 



0.0 


45-37 2li 2 C B H 4 4 


-3H,0 


1 .27 


45 '41 " 




2.8l 
2.84 


45.75 "+ LiHC e 
40.55 LiHC a H 4 4 . 


^6' : 


3.46 


36 . 25 " 




4.15 


32.40 " 




7.15 


26 . 09 " 




9.6l 


22.45 " + ^J>^8 


^4^4 


8.67 


20. 39 N?^8"44 




7.45 


16.55 " 




5.58 


11.06 " 




3.92 


5.83 " 




1.97 


2.28 " 




0.30 


0.0 





14.01 

3 13.32 
10.56 

3-34 
0.68 

Results at 50 



25.56 
19.39 

8.87 

3.22 

0.0 



Results at 25 



0.0 



.38 
,60 

,20 
51 
79 



45.20 2Li ? CJ! 4 4 .3H p O 



9.08 
11.39 



45.15 

45,19 " + LiHCJI.O .aP 

38.13 LiHC 8 n 4 4 .aH ? 

34.07 " 

32 . 36 " 

28.23 " l -7S o.o 

EQUILIBRIUM IK THK SYSTIM LITHIUM PHTHALATI, MAGNESIUM 
PHTHALATI AHD WATER. 

(Smith and Ely, tgm.) 



0.0 


46.08 


3.73 


46 . 1 


6.40 


q6.oo 


9.97 


46.01 


12.43 


19. 3-2 


15.07 


34.77 


18.92 


30,0$ 


21.78 


28.29 


24.00 


26.69 


1S-20 


15.28 


11.48 


10.80 


6.8l 


5*10 


4.75 


3.38 



a 



(tea, per 100 t^a. aat. aol. 

r Mgc a H A o^ Tno/ 8 

844 *. o ' 

Results at 25 



OBIU. per 100 Hiag. auu tol, 

. mmmm^p-a* m^am.a*^mn,~mam:/\- ..> %< - I- ' * ^ 

Results at 25 (con. I 



0.0 

7.52 
12.98 
16.39 
19.27 
19.97 

20.43 
20.96 
22.40 
23.06 
25.31 



45-2*, 
41.12 
36.72 
34.50 
33-05 
32,50 
29.53 
26.88 
21.78 
19.63 

14.86 



"4-aMgCJL 



31*09 


4S5 


34.14 


0.0 


Results at 


50 


f b o.o 


46.01 


6.97 


41.76 


18.32 


35*33 


26.06 


3KOS 


34.75 


17-49 


36.10 


1U74 


40.31 


3.18 


42.28 


0*0 



Li LITHIUM 



QC)6 



CH 



LITHIUM Racemic and Laevo MANDELATES LiC Q l! 7 3 . 

EQUILIBRIUM IN THE SYSTEM LITHIUM (r) RACIMIC MANDBLATB, RACEMIC 

MANDELIC ACID AND WATER AT 25. 

(Ross ana Morrison, t9ZW.) 



Otas. per 100 BWS. 


sat. sol. Solid 


0. ptr 100 AS. 

-.* , /V , 


sat, sol. Solid 


'"Ws 


"uFH"o^ x Phase 




LlCgH^O^ Ph&se 


0.0 


4.9 Lic e H 7 o,, 


13*7 


3-3 Ul 


0.9 


4.7 " 


14.6 


3-2 " 


<J.O 


4.7 


111* 1 


3.2 


4.7 


5.0 " + 1 . 1 


16,2 


3-1 " 


6.6 


4,2 1.1 


18.2 


* , M 


8.3 


3*9 


i) . 


3."o 


99 


3-6 


20.1 


3.0 " t HC fl H 7 0, 


11. i 


3-6 


18.8 


1.6 HC H ? 0, ' 


13.0 


3-3 


16.9 


0.0 



1.1 =LiC fl H 7 O s .HC 8 7 3 . 

EQUILIBRIUM IN THE SYSTEM LITHIUM (-) LAIVO MANDILATE, LABVO 
MAKDBLIC ACID AND WATIR AT 25. 

(Boas, Morrliitm ana Jotostant, 19^7.) 



Tuna, per 100 i 


ma. iac. aol. 


o nu 


ftes, pff 100 MB 


. Ml. SOl. 


Solid 


,__-_ 


(-)UC p HX 


Hui.'u; 


/ 7-)HC J| H 7 6 !t 


'" )W Ws 


Phauit 


0.0 


8.6 <- 


me H o 


10.6 


3.5 


1 .1 


1.0 


8-S 


M 


n. g 


3*4 


i 




8.6 


H 


10.3 


3.4 


<-IHC 9 H,0 


2^6 


5.6 


i a 


10.3 


2,6 


II 


S-6 


4.0 


H 


10.0 


1.7 


it 


6.9 


4.0 


H 


9.9 


0.8 


It 


9.2 


3.7 





10,1 


0.0 


fl 



1.1 = I-) LiC B H 7 0,.HC 8 H 7 3 

DiLITHIUM (/ CAMPHORAT3B C tw HiALi s . 

SOLUBILITY IN AQUEOUS SOLUTIONS OK CAMPHORIC ACID AT i3.5-x6 

AND VICE VERSA. 

and Landrku, iMt i ) 



CiHi(COOH)t 



Cms. per 100 Cms. Sat. Sol. 

Solid Phase. 

Camphoric Acid 

a a 

Monolithium Tctrucamphoratc 

* i* 

** Dicaniphoratc 

" ii 

44 Camphorute 

Dilithium Cumphorate 

Thcjnixlures were kept in a cellar at nearly constant temperature and shaken 
from time to time until equilibrium was reached. Additional results at i7-23 
arc also given. 



C|H M (COOH),. 


CioHiAu] 


0.621 


O 


2. 02 


3-77 


3-2S 


10.63 


3-Si 


12. 6l 


3-99 


20.56 


3-43 


24.69 


2,87 


37.16 


o 


40.80 



907 LITHIUM 1 

LITHIUM LAURATE, MYRISTATE, PALMITATE and STEARATE. 

SOLUBILITY OF EACH OF THESE SALTS, DETERMINED SEPARATELY, IN 
SEVERAL SOLVENTS. 

(Jacobson and Holmes, 1916.) 

Li laurate = CuJH^sCOOLi. Li myristate CuHjrCOOLi, Li palmitate 
CH 3 (CH 2 )i4COOLi and Li stearate = CHiCCHjJwCOOLi. 

Excess of salt shaken with solvent for 2 hrs. in all cases. The sat. sol. was 
analyzed by evaporating to dryness and weighing residue. 

Cms. of Each Salt (determined separately) per 
xoo Gms. Solvent. 





" 


Li 


Li 


Li 


'- ^ 
Li 






Laurate. 


Myristate, 


Palmitute. 


St curate. 


Abs. Ethyl Alcohol 


20 


0.403 


0.194 


0.096 


O.O72 




25.4 


0.447 


O,224 


0.1x8 


0.089 


<t 


35 


0.546 


0.278 


0.142 


0.106 


<t tt 


5 


0.782 


0-435 


o . 248 


0.20O 


tt 


65 


I . 149 


o . 669 


0.391 


0-333 


Methyl Alcohol 


15.2 


3-159 


1,346 


o . 6 1 6 


0.349 




2 5 


3 773 


i. 680 


0.771 


0.439 


it tt 


34.6 


4-597 


2.193 


i .086 


0.658 




So 


6.088. 


3.281 


i .652 


1.057 


Water 


16.3 


o-i54 


0.027 


O.OIO 


0,000 


tt 


2 5 


0.187 


0.036 


0.015 


0,010 




35 


o. 207 


0.042 


0,015 


0,010 




50 


0.280 


0.062 


, . , 




Ether 


15.8 


o.or i 


0.013 


0.007 


0,011 




2 5 


0.006 


0,004 


0,007 


O.Ol I 


Amyl Alcohol 

tt it 


16 


0.073 


0.029 


O . 1 {) 


o,or r 




2 5 -7 


o . n i 


o 046 


0,032 


O.02K 


tt te 


35 


o. 126 


0.062 


0,033 


0,031 




49.2 


o . 203 


o. 109 


o , 069 


o 060 


Chloroform 


XS,2 


0.006 


0.004 


0.004 


0,004 


Amyl Acetate 

it U 


H-5 


0.068 


0,037 


0.038 


0.034 


tt tl 


25 


o . 064 


0.034 


0.024 


0,029 




35 


o . 06 1 


0.044 


0.037 


o , 03 1 




50 


o . 06 1 


0.045 


0,036 


0.044 


Methyl Acetate 


24.5 


0,026 


0.013 


0.015 


O.OI2 


Acetone 


15 


0.300 


0,413 


0,434 


0.571 


u 


2 5 


0,376 


0.447 


0,508 


o . 706 




35 


0-430 


0.502 


0.537 


0,663 


lithium acetate to the 


alcoholic sw; 


epared by 
ilutions of 


adding ih* 
the rt*8fx*ct : 


ive fatty a 


cids. Tht* 



resulting pmapitates were dissolved in lxilin K alcohol 
drie S d Ver " lght '" " C00 ' Place ' The 



the so uti,, n allo 
were 



Li LITHIUM go8 

LITHIUM LAURATE, MYRKTATE, etc. 
SOLUBILITY IN WATER AND IN ALCOHOL OF d** 0.797, AT 18 AND AT 25. 

(Fartheil and Ferie, 190,1.) 



Cms. Bait per 100 cc. Sat. Solution in: 



Salt. Formula. Water at Alcohol at 



18". 23*. xii e . 25. " 

Stearate CirHasCOOLi 0,010 o.on 0.041 0.0532 

Palmitate CisHsiCQOLi o.oii 0.018 0.0796 0.0956 

Myristate CialfcCQOLi 0.0232 0.0234 0.184 0,2100 

Laurate CnH^COOLi 0.158 0.1726 0.418 0.4424 

Oleate CnHsiCOOLi 0.0674 o.ipo 0.9084 i.oio 
LITHIUM Platino CYANIDE Li t Pi (GN .u.f H,0. 

SOLUBILITY OF LITHIUM PLATXNOCYANIDK IN WATER, 
(Terry and Jolly, 1913.) 



Sins. U s Pt<O' ( tlms. 3 

t". ,>er JOOfras. 11,0. t. |r too gain. II, O'. t". Pr too m<, H,O, t s . per lio'gina! H 0* 

o.o... io5.o 3o.i... i5->,.3 4-^-' i6o,3 5.i.,, 1750* 

16.3... i39.5 3o.5.:. (56. i 42.5... 160.5 5S.o... i8->.!o 

22.2... i4i.5 3i.5... iSu.o 4-A-7-. 8i.u 55.x,... nS.'s 

CN 23.0... 153.5 :h.2... \f>*..\ 43.1.. iH8.-i 60.7.,, 178.0 

24 - 1 1 44 8 34 . 9 . . . 1 6T) .6 4 3 u . . . i CM ,3 (4 , 8 . . , 1 85 7 

25.o... 144.7 'i5.o... 1 54.(> ,f).<... 196,0 6(>.o./ 'i(j5'.l 

25, 7 ... r-)3.o 35.8. . 155.6 ,(:>.;... ifo.o 71.0...' 2 n4.'o 

25.8... i/j(>.,i 37.3... 173.0 46.6... 176.1 72 (tr.pt.) 

26,5... 147.5 38.0.,. i55.3 47. i,.. 186.0 78. a... 2137 

26.8... iSi.a 388... i58. 48.0... i 7 3. ft8..., ^o!i 

28.5... 148.5 39.1*... 1.54-1 /i9.<>fr.pt.) Htj.H... u'J8 7 

'^.9. 5 (tr.pt.) 39.5 (ir. pr.) 49- '*... i7'J.i 

EQUILIBRIUM IN THE SYSTEM LITHIUM PLATINOCYANIDE, 

POTASSIUM PI.ATKNOCYANIOK AND WATEK AT 44. i. 

(Ti*ry nd Jolly, 1933.) 

Cms. per (00 gms. Gm. prp two g m*. 

sat. sol. Mft t. wl, 



Solid PhM. Jt4,I*l|N),. X t FlftlNl,. Solid ,. 

5g. a o.o Lit.PtCCNH.tHtO ug.3 18.7 LiKPi(ON)7."aH.O 

54.2 1.7 LiKPtlCNh.ul^O 28.7 iH.a K 9 Pt(CN),.3H 2 

54-1 a. a tt7 .3 16.1 

te- 1 a-7 3.o 19.8 

45-9 4-4 > TA.O 19.4 

38-9 9- 19-3 o. 

3^-5 11.2 > jo. 'i1,6 

34 I J* .3 6.1 'Jl6 , ') n 

CNS 3 2'J l3 -y w 4-B a6.\j 

tto.5 ih. > ,. -*H (i i 

LITHIUM Thio CYAN4TE LiSCN.2H f O 

OF LITMI0N TIOCAirATE IN VATBR. 



Ctaa. L13CH per iia p ote. UtfCN ptr Solid 

loo m* sat. aoi, pftwt 6 too ^^ mlm mlf 



20 53. a LiSOI.aH^O 31, LiSCN.alLO * LtSCN 

2 5 5H.5 " 3S 58.8 liSCN 

3 $ 6 *7 " HO 60,4 H 



909 LITHIUM I 

LITHIUM CAEBONATE Li 2 CO 3 . 

SOLUBILITY IN WATER. 

(Bevade, 1885; Flttckiger, 1887; Draper, r88?.) 

An average curve was constructed from the available results arid the following 
table read from it. 

Cms. LigCOaper too Gms. Gms. Li 2 C( ) 3 JHT too Oms. 

to ' Water. Solution. " Water. Solution. 

o 1.54 i-5 2 40 1.17 1.16 

10 i-43 *-4* 50 *-o8 1.07 

20 c-33 1.31 60 i .01 i .00 

25 1.29 1.28 80 0.85 0.84 

30 1.25 1.24 100 0.72 0.71 

Density of saturated solution at o - 1.017; at 15 1.014. 
More recent results at o agreeing with the above are given by Rosen- 
heim and Reglin, 1921; and at o and 100 , by Kraus and Burgess, 1937. 

Determinations of the equilibrium in aqueous solutions of lithium 
carbonate and bicarbonate in relation to the partial pressure of the 
carbon dioxide in the gas phase in contact with the solution are given 
by Walker, Bray and Johnston, 1927. 

SOLUBILITY op LITHIUM CARBONATE IN WATER UNDER HIGH 

PRESSURES op CARBON DIOXIDE. C 

A platinum lined autoclave was used and the mixtures shaken i hour 
and allowed to stand 1/2 hour before removing a. .^impie for analysis. 
Lithium carbonate goes into solution in water in presence of 00 p AS* 
bicarbonate. Such aqueous bicarbonate solutions <ire stable above -13 
only under a C0 ? pressure of more than i atmosphere. The result.* are 
presented both in terms of gms. of Li^CO^ (shown in parentheses in the 
following table) and of LiHCO., per 160 gms. sat. solution. 

Pressure of C0 ? .^^J^I^lJd!^ ? ^ r lo *** **n*rtLu wiullon *b: 

In Atmospheres ~ -~-~ ~~~ ^^ ,,.,^g.. OT ....,, ..^ 



1 


22,71 (12,36) 


21.25 (11*36) i6.x: (8.77) 


3 


22.71 (12.36) 


22. tit (12.30) """"* 


5 





22. <f t (12.2O) 3i.V> Ul.6a) 


8 





2U'i6 (11,62) 


10 





, , 


13 





_ 


16 





^ 


20 





_ 


30 





- 


34 





^ 


SO 





* . 


if C0 g 


'tan. UhCO ti 


^r too Htfa. Mmr^ud MluUon &u 



Pressure of CO, 

In Aunospherea / o 

1 HI- 13 (7.69) 10,56 (5.7S^ B.S5 (4.65) 7.U M.99) 

5 ' 16.96 (9.23) 12.52 (6.82) 8.62 (if, 69) 

8 19.91 (10.83) - 

10 19.9^ (10.83) 14*90 (8. n) 8.68 (4.7-8) 

13 16.19 (8.81) 

l6 17.39 1 9. i|l) 

20 17.29 (9.ai) n.<i8 (6.2*0 ?,;, tn.io) 

30 ~ u.2H (6.66) 

3 ~ 12.23 (6,65) 

100 gms. II ? dissolve $.501 gms. LH1CQ R at 13. <BevAde" iHB*/. ) 



Li LITHIUM 910 

SOLUBILITY OF LITHIUM CARBONATE IN AQUEOUS SOLUTIONS OP 
ALKALI SALTS AT 25. 

(Geffckm Z. anorg. Chem. 43, 197, '05.) 

The original results were calculated to gram quantities and plotted 
on cross-section paper. The figures in the following table were read 
from the curves. 



_ -. w urams 1*12^-^3 I*r Juuer m Aqueous rxuuiums 01: 


per Liter 


* KClOa. 


KNO 3 . 


KC1. 


NaOL 


K 2 S0 4 . 


Na 2 S0 4 . 


NH<n. 


(NH<) 2 M) 4 . 


O 


12.63 


12.63 


12.63 


12 . 


3 


12 


63 


12.63 


12 


63 


12.63 


10 


12.95 


I3-05 


13.10 


*3- 


4 


13 


9 


14.0 


1() 


.0 


20-7 


2O 


13.10 


13-3 


I3-S 


*3- 


9 


14 


7 


15.0 


19 


.2 


25.0 


3 


J 3- 2 S 


13-6 


IS'* 


14. 


3 


15 


4 


16.0 


21 


s 


28.2 


40 


13.40 


13-3 


I4.O 


14. 


6 


16 


.0 


16.6 


23 


-3 


30 -'8 


60 




13-8 


14.2 


14. 


>5 


16 


9 


17.8 


26 


.0 


35-2 


80 


. . . 


13-6 


14.0 


14. 


<4 


17 


7 


18.6 


27 


.6 


3^5 


IOO 


. . . 




13-9 


14. 


2 


18 


.2 


19.4 


28 


4 


41.0 


1 20 


* 


Z 3 -3 


13-7 


14. 


O 


. 




19.9 


28 


7 


42.6 


140 


. . . 


13.0 


13-3 






. 




20.4 


28 


.8 


43-5 


170 




12.6 














28 


9 
















2OO 




12 .2 














20 


.0 





CO TOO g;ms. aq. alcohol of 0.941 Sp. Or. dissolve 0.056 gm. LiCO s at 15.5. 

OneTiter sat. soK in water contains o. 1 722 gm. mohs. I 2.73 K ma. LijCOa at 25. 

(Ageno and Valla, mil,) 

SOLUBILITY OF LITHIUM CARBONATE IN AQUEOUS SOLUTIONS OF ORGANIC COM- 

POUNDS AT 25. 
(Rothmund, i^oH, 1910; aee atao Traubc, 1909.) 

The solubility in HaO 0.1687 mots. Li-tCOa per liter 12.47 gins, at 25. 

dm, Mols. LijCOj JHT Liter in Aq. Solution of: 



Aqueous ooiuuan 01; 


o.x a 5 
Normality , 


Normality. 


Normality. 


I 
Normality. 


Methyl. Alcohol 


. . . 


o, 1604 


0.1529 


0.1394 


Ethyl Alcohol 


O.l6l4 


O.J55S 


0,I47 


o . i 203 


Propyl Alcohol 


o. 1604 


0.1524 


0.1380 


0.1097 


Amy! Alcohol (tertiary) 


0.1564 


0,1442 


0.1224 


0.0899 


Acetone 


O.16OO 


0.1515 


o , 1 366 


O.U04 


Ether 


0.1580 


o. 1470 


o. 1300 




Formaldehyde 


0.1668 


O.I6S3 


o. 1606 


0.1531 


Glycol 


0.1660 


O.1629 


0.1565 


0.1472 


Glycerol 


0.1670 


o. 1647 


o, 1 013 


0.1532 


Mannite 


0.1705 


0.1737 


0,1778 




Grape Sugar 


0.1702 


0.1728 


0,1752 


0.1778 


Cane Sugar 


0.1693 


0.1689 


O , ! 66 1 


0,1557 


Urea 


0.1686 


0.1673 


o , i 643 


o. 1605 


Thiourea 


0.1667 


0.1643 


o, 1600 


0.1523 


Dimethylpyrone 


0.1562 


o. 1460 


o. 1280 


0.0992 


Ammonia 


0-1653 


o . 1 630 


0,1577 


o, 1466 


Diethylamine 


0.1589 


o. 1481 


o , i 283 


0.0937 


Pyridine 


0.1592 


0.1503 


0.1347 


o, 1091 


Urethan 


0.1604 


0.1525 


0.1377 


o. 1 1 13 


Acetamide 




0.1614 


0.1520 


0.1358 


Acetonitrile 


0.1618 


0-1556 


0.1429 


o. 1178 


Mercuricyanide 


0.1697 


0.1704 







Freezing-point data for mixtures of LitCOi + Li s S() 4 (Amwlori. 1 



LITHIUM Li 



SOLUBILITY OF LITHIUM CARBONATE IN AQUEOUS SOLUTIONS 
OF ACETONB AT 17.6. 

(Hartley, 1931.) 

Mols. (CH 3 ) 2 CO per l.o Mol. Mol*. U ? CO., per I.Q Hoi. 

(CH^CO + H ? UgCOj * (CH 3 ) p CO * H ? 

o.o 0.00331 

0.0326 0.00211 

0.0668 0.00105 

SOLUBILITY OF LITHIUM CARBONATE IN AQUEOUS SOLUTIONS 
OF SEVERAL ORGANIC COMPOUNDS. 



The solubility in water alone is 0.1691 gro. mols. Li ? C0 3 per Liter. 

Qm. Hols. Ll^CQ^ per liter in AQ. Solution of: 
< ~~*"~~~' ' ""^ ^^~~ 



Aqueous Solution of: ' 0.005 < ~~*0^o7Be"~~~0'. 04l ' ""oTWWT^ ^TTTTI'r^ 

Nomallty Nom&ltty Normality Norwallty Normality Normality 

Paraldehyde - - 0.16^9 0.1573 0.21167 

Iso amyl alcohol 0.1621 Q.1SS9 "~ 

Hexyl alcohol 0.1666 0.1640 

Octyl alcohol 0.1683 ~~ 

Fusion-point data for mixtures of Li p 00 3 Na p C0 3 are given by Skaliks, 
1928.) 



LITHIUM OXALATE Li 2 C 2 O 4 . 

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 r and the solutions coolt'tl 
in a thermostat to 25. 
Cms. per roo Cms. Solution. Mols. per 100 Moli. H g O. 

' " 



10.20 ... 2.274 ... HaCA 

' 2 '*V ' 622 HaCA.HtO and HLICA.H.O 



8.08 3.18 1.823 
2.60 5.03 0.563 



.633) 
5.962 \ 



and 



5-87 ... 1.901 LiiCA 

loo gms. aqueous solution, sirnultaneously saturated with lithium oxalate and 
ammonium oxalate at 25, contain 5.75 gms, LiC 2 O + 4.8 gnm (NH 4 )CV>4. 

w, 1905.) 



Li LITHIUM 

LITHIUM OXALATE 



EQUILIBRIUM IN THI SYSTEM LITHIUM OXALATI, ZIRCOHXUM 
OXALATE AND WATER AT 19. 



The solid phases were of uncertain composition since the zirconyl 
oxalate apparantly hydrolyzed, yielding mixtures composed of the oxalates, 
oxalic acid and water. 

Gtaa. per 100 pis.^smt. solution Qtea. ptr 100 

COO 



r Ll g (COO) 2 


*2rofOoo^ 


' U 8 rooo) t 


-mrm^ 


LT ^ mr ^ 


*ro(cooy 


6.06 


0.0 


6.89 


3-41 


7.10 


5.35 


6.37 


0.81 


7.15 


3.70 


6.20 


6.00 


6.66 


1.56 


7.43 


3.82 


5.63 


6.91 


6.50 


1.82 


7.52 


493 


4.20 


7.72 


6.56 


2.05 


7.70 


soi 


3'S3 


8.2(| 



LITHIUM CHLORIDE LiCl.H^Q. 

SOLUBILITY op LITHIUM CHLORIDE AN WATER. 

The results of Huttig and Rensher, 1934; Benrath, 1927 i932^J Ueacoa, 
1927; Friend and Culley, 1931; Basset t and Sanderson, 1932; Appleby and 
Cl Crawford, 1934; and Friend/ Hale and Ryder, 1937 were plotted and from 
the average curve, the following values were taken* 

0. of 3fc. LiCl pir -Solid 

uu... Ml. 100 $* *! Ml< ^&se 

1.131 53. 8 LiCl.HjQ 

h. f i47 56.1 " * LiCl 

56.8* LiCl. 1^0 

1.347 56.2 LiCl 

56.7 

X.B44 57.2 

57.6 
1.339 58*0 

- 59.3 

Kits 

Appleby and Crawford give the transition points as i*>.i and 93. 





* of 


Ona. L1C1 per Solid () 




sat. sol. 


100 ia. *at, m ~ 


u. pnwt 





1.268 


40.9 


LiC1.2H f O 80 


5 





42.0 


90 


10 


1.279 


42.7 


11 fif. i 


15 


_ 


43-8 


97 


18 

25 


.5ta&pUi.293 
1.296 


45-35 
45.8$ 


"+ LiCl jyDoS 
Li Cl . H f 100 


30 





46.3 


11 HO 


40 


1.303 


47*3 


M 120 


50 


1.308 


48.3 


" 130 


60 





49.6 


11 140 


70 


j i i 


51-4 


11 l6o 



913 LITHIUM L 

LITHIUM CHLOKIDE Li Cl. 

FREEZING-POINTS OF MIXTURES OF LITHIUM CHLORIDE AND WATKH 

Results of Results of 

Klcia and Svanborg, 1920. Umldmsh, IJUH. 

Normality of A<I. UCI. F. pt- of solallon. Urns. LI 01 pnr lOOftnis. H a (>. F. pi. of sol.iUou. 



. 

1 2 5 o . c) 1 6 i o . 68 

<K5o... 1.807 iS.o.f 

iB. r )8 



The following determinations of the transition points of Lithium 
Chloride in Water, made by the freezing-point method, are given by 
Httttig and Steudemann, 1927- 

QBS. L1C1 PJE loo p>a. 8oHdi 

t ^ no aiftu solution 1 Phat 

-80 33-9 25-3 J ce * LiCl-sIi 

-68 40.3 28.7 LiCl.sH.O * LiCl.3H p O 

-20 ' 58. <i 36.9 LiCl. 3 H 8 * LiCl.aH 

4i2. 5 68.0 40.5 LiCl.aHjO * LiCl.H^O 

100.5 130.0 56.5 LiCl.H,0 * LiCl 



SOLUBILITY OF LITHIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC 

ACID. 

Results at o. * (Engel, i8S8.) Results al 25. (Hem, 0u-u.) 

Gms. per 100 cr. Sat. Sol. *..**. Onw. pi" *oo cc, Sat, Sol. 

' " 



' LiCl. 


HG: 




' LiCl. 


HCI; 


Si 


o 


* 255 


57-4 


o 


41.4 


8.2 


1.243 


56,87 


^ '3 


28.5 


24.1 


1.249 


S3 *&4 


3,84 


24.6 


29-5 


1 .251 


51.98 


^43 



EQUILIBRIUM IN THE SYSTEM LITHIUM CIU.OIUDK, LITHIUM SUI.I-'ATM AM> WATI:II 

AT 30. ( Schrtiiruiinakcr;' und Kayt<r, IDIB, ) 
Cms. per lOOgms. sut. sol. Gm?. por )(M)j|M,fi{ii,&ul 

LiCl. Li, SO,, Solid Plwiuc. MCI. M.;S(>,. Suit, l^l'l. ,.-. 

46.io o.o LiCi.H 2 C> 8.07 iu,-/o LitSO^.I^O 

45.97 o.o -t-LisSOiHgO 5.74 r>.7i 

30.74 o.o (JiSOi.HiO 3.t)H 18.85 

a i. 04 i. 08 2.76 uo./j'J > 

i5.3o 4*4^ v> 0.96 u3.(5o 

12.06 7.48 o.oo yt.0,7) 



Li LITHIUM 

LITHIUM CHLORIDE LiCl. 



Cl 



20 



35 



i THE SYST*M LZTMZUM CHLORIDE, MAHGANISI 
N WATIR. 



f tar* ft. 1934ft. ) 



(tes. per 100 
gnus, M th ** id 


flfci. ptr too 

1 ^a- MJ^. i0i. Solid 


/ HnaJ~' 


uei ' ** 


'^n f 


' urp ^wt 


0.0 


40,51 LiCl.aHjO 


IS 39.07 


17.66 MaCl.aH.O*MnC] 


0.54 


40,33 H * 4.1. 10 


w 11.00 


11.76 MnCl .48 


2.35 


36,77 4.1.10 


* 13.71 


10.73 " * 


3- $6 


35-33 " 




0,0' H 


8.6a 


32*30 M 


60 0.0 


49,61 LiCl.H.O 


10*19 


31.10 " 


" 1 . 17 


48.lt8 


11.54 


30.24 " * 1.1.5 


4.11 


47.10 " 


11.63 


30.18 1.1.5 


S-S! 


46, SO " * 2.1.4 


13.43 

13.45 


28.* 60 M * HwCl .*$/) 


- ill! 


41*07 3.1,4 

37*74 H 


12,48 


25t40 MnCl.4ll,0 


" 17.91 


"S|. 8| H 


1*1*1$ 


23.13 M 


" 10. 5 


11.11 1.1.3 


37.91 


8.84 * 


" 31.71 


39.09 MoCl ? .2HJ) 


38.86 


0.0 H 


w 11 * m 


15.63 H 


0.0 


45.38 LiCl. alLO* LiCl, M, 


P H 41.58 


B.14 


0*81 


44-67 LiCl.HjQ * 4. 1. 10 


M 51.60 


o * ci * * HnCl \$ 


0.86 


44*53 4.1.10 


Ho o.o 


^j.8 LiCl.H^O f 


3*73 


39- a6 " 


" S-J5 


4947 w 


9.09 


34.82 " 


7*78 


ft- 11 N * 2,1.3 


14*39 


tl M< ** 


" H 94 


47-10 3.1.3 


16.47 


30. tl w 


* V W 


46.17 M 


17.25 


39.6s w - 1.1.5 


" 13.&6 




i8.a6 


28.50 !.!$ 


** 17. 8a 


16,79 1.1. a 


19.13 


27.65 H 


M Ji *^j 




22.2$ 
31*28 


36,74 HaCl,.afLO 

23.82? w * HodL^Hjp 
23*47 HaClp4HpU 


w 37. 5a 

11 15.11 

" 5^.03 


a'a.ai "+MftCl f .aHj 
i5.oa MoClj.aH f O 


28.75 


11*51 w 


00 . O 


55^84 LiCl 


42.36 


0*0 " 


** ft * ;*? 


51.06 w 


3$S 


4Si4 iiCLtf/l * ja. 


** 7* jM 


50.75 w * a. i.a 


5.48 


40-51 JM-* 


f< H.Ki 




10.66 


1S*93 ** 


" 1 1 * J 1 


44. j6 M 


12.99 


34 * 3$ ** 


" 7.Ri 


1^.77 


18.86 


*30.08 w 


** mJn 


17.45 * * 1.1.3 


20*29 


39.11 " * NoCl^.jH f () 


** J7^J 


to. aa 1*1.3 


21.57 


36*40 MCl.alt f O 


** M.77 


j^.fta M tMnClg.aHj 


28.77 


17.98 ** 




15. Ho MCl f ,aH f O 






" ^ | 4O 


u.o w 



MnCU.2 



.1*5 z LlCLHftCl p .5i 0; 4*1. to - iititl.HiiCIy, idll J); j.i.j : 
l.-'aH H* * t. r f iPi Mf*i ., y rt, , .. ^ t ii*i 6-ifM -.** A 



1 .1 .3 " 



Incomplete <Uu *r* givta fr ib* liiuihrm^ AI ui* 17.5 22> 

27 43 > 45 t 65* 7d 75*, fO e Ati * 



9 IS LITHIUM LI 

SOLUBILITY OF LITHIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE 

AND VICE VERSA AT 25. 
(Smith, Elgcrsma and Hardenberg, 1921.) 

The saturated solutions were analyzed by a viacometric method and also by 
a modified synthetic method. 

(Sins, per toogms. MI. sol. Cms. per 100 g m. cat. sol. 
M Cl. Na Cl. "tl a. " ~Na7?l. 

45. 8 o.o 33.5 0.3 

45-5 o.5 3r.6 0.8 

4'- 3 0.4 24.9 a 3 

4o. i o.<2 17.4 7.3 

36.8 o.3 16.9 ..{ 

35.7 o.3 6.5 in. o 

33.5 0.4 o.o *&.<} 

EQUILIBRIUM IN THE STSTBN LITHIUM CHLOHIDB, NICKEL CIILOHIDE AND WATER. 

(Benrath, 



Ota. ptr 100 m*. aac. aol. Solid (tea. ptr 100 



b 


' MiCL ? 


LlCl ^ Phaae 


& 


' IdlCl 


u^,^,. , 


"^ Pfc&a 














Cl 








40.51 LiC1.2H g O 


25 


6.98 


30.96 


NiCL. 4HJ) 


" 


0.38 


40-42 " + 4. 1.10 


11 


10. 23 


26.90 


M 


* 


2.45 


36.24 4.i.io+NiC]^4li 


Lp " 


17.13 


19*52 


n 


n 


3.14 


33*58 NiCl ? .4H ? 


II 


27. S5 




H 


H 


4.83 


30.57 


11 


26.79 


10.58 


NiCl .6H 


it 


9.08 


22.64 NiGlo*6HpO 


H 


33-56 


4-94 


i 


n 


34.08 


0,0 " 


M 


39.58 


0.0 


M 


17-5 


0.0 


44.61 LiCl p .2H ? 


50 





48*18 


LlCi.Hjp 


11 


0.28 


42.6l '4*1*10 


M 


0.26 


48,11 


"* 2, 1.4 


M 


0.40 


43.97 


H 


1.11 


43-36 


2.1.4 


" 


2-33 


38.78 H 


M 


3*59 


39.17 


n 


11 


3.84 


36.83 NiCljj.aHjpCK 


H 


2.84 


40.24 


NiCl .2H 






NiCl ? '.4H ? 


n 


3; 87 


37.72 


n 


" 


9-32 


26.65 NiCl f .4H p O 


II 


10*, 9 7 


28.39 


M 


H 


13.64 


22.04 " 


II 


15,12 


24*60 


w 


" 


18.49 


17.65 " 


n 


29*44 


12.78* 


H 


11 


15.99 


19.73 NiClg.6H g O 


n 


18.25 


ai,6s 


NiCl .tiH 


" 


20.56 


14.69 " 


n 


22.43 


17.38 


H t f 




37.07 


0*0 " 


11 


27.69 


12.70 


H 


25 





45.90 LiCl,H 2 


H 


35-05 


6.60 


H 




0.21 


45-17 " * 2.1.4 


n 


40.20 


2.38 


11 




0.50 


42.92 2.1.4 


it 


43-17 


o.o 


n 


11 


2.46 


38.93 H 


99. 


5 0.0 


53-84 


LiCl 


" 


3.11 


38*17 "* NiCl ? .2R^( 


"\ H 


o-SS 


55-50 


H * 1.1.2 




3.18 


37.85 NiCl^.aHj.O 


M 


0,72 


54*66 


i.i. a 


ti 


3.46 


3756 " 


ri 


1*42 


48.66 


M 




4.43 


35-95 " 


if 


5*35 


40.58 


""NiCL.rf.0 


" Metastable 
4.1.10 = 4LiCl.NiCl 
2.1.4 = aLiCl.NiCl, 
1.1.2 = LiCl.NiCl^; 


r loH g O 

2ll g 6 


H 

ft 

II 


8.49 

14.86 

28.85 
36.30 
46.71 


34*24 

26.71 
14.49 
8-97 

0.0 


NiCl .aH f O 

H 


Incomplete results are also given for 

uO.*. 6n* AnH cr 


the 


isotherms at 


20, 30 


. 15, 



Li LITHIUM qi6 

LITHIUM CHLORIDE 



RQOIMBRXWM IN IMS STSTRH LXTHXNH CHI.ORXDI, \HMOHIA 

AND WAXES AT aj-as . 

'folltn* iftfl CMMitm, to**.* 



per 100 ^ ^ tiwu Pr 100 ^ ^ *!*. p*r 100 

M*. Ml. Ml. 



45.4 o.o LiCl.Il t O 51.9 16.70 UtU.NH, t^.n ^. 7 UC1.3NH S 

(j6 . 7 3.1 '* <J4 7 30 , ** 4 * * S-" 1 *5 . 7 H 

48.1 7-9 " 570 31.64 " Wl 15.8 M 

50.84 13.88 " $3.57 37.11 " W*U 0.6 M 

50.73 14.86 " 46*1 ia,c> LiCl,;|NHj 17* 

50,81 15.2 



The authors also give vapor prt?Hur^ w^AriunMnonui for the above 
system at 2$^ and for the system UCl * NH,, At iht temperatures o 
33% 4S*a. 54. 5. 5B*i <t6.ii, ?n.6 .m.fH6.>. 

100 gms. Liquid Ammonia ditisolvc o,riB ui. LuH *ii -H-9 (Johason 
and Krumboltc, 1933.! 
100 gros. Liquid AmwoniA rti**olve i.^i jfR. LiCl At o**. (Li&hard and 

Stephaa, 1933, 1934* J 

BQOXLZBKXtm I THE StSTIW LlTKXUM CtaftftX D f LlAD CHJLORXDI 

AT 3S 



Ona, per 1000 pui* KJ9 SOII4 Qfti* pr |Hi. ,, ,<Uli 

' tlfl ' "" W8T.''"'"N 



830.5 o.o UCl.H f O aai.6 1*61 PbCl,, 

830.0 17.2 w 156.2 a.^ft w 

835*0 31.0 w 7S.W 1.51 W 

835.0 72*0 M 41.77 1.19 " 

834*9 101.6 ** * PbCl ? 31.64 l.^H " 

794*1 1034 PbCl^ 7l6 3.$S '* 

621.8 94.43 ** ' 6*67 368 * 

4S3*9 48.71 w |.88 a.^n w 

329.2 16.36 ** 0.0 10. 7 " 

OF LITHIUM CRUUIXDI IN A^TKWS S< 

or ETHYL ALCOCIL AT 35. 

i<i Ki'olauu., ifK.) 



n3. per 100 gp. ri(U, wul. teUd QM, pr IW W. Mt. Mi,, Solid 

rt'/\.rw..,. 



45.94 o.o tlCl.H/) 37.10 56.4a LiCi.H f O 

4^.90 441 H 35*41 60*34 " 

41.88 12.92 w 23.09 66,77 " 

40.6$ 14.49 w 33.41 68.96 H * ^ iCl 

37.02 24.39 M 23* 18 72. 98 kiQ- 

34.17 34.24 '* 33.1,1 74*2M| M 

30.02 47.43 H 30. 18 79.82 w 



917 LITHIUM LJ 

SOLUBILITY OF LITHIUM CHLORIDE IN AQUEOUS SOLUTIONS OF ALCOHOL AT 25. 

(Pinar de Rubies, 1913-1914-) 

The LiCl was determined by titration with AgNO.^ Solutions saturated by 
constant agitation for many hours. Solid phase, LiCl.HaO for all mixtures. 
The anhydride, LiCl, separates only from the most highly concentrated alcohol 
solutions. 

Gms. per too^Oms. Sat Sol. Gms. per too Cms. Sat. Sol. 

TjH B OH. " LiCl. "' 'C S H 6 OH. ' LiCl. * 

o 44-9 50 25.75 

10 40.9 60 21.6 

20 37.25 70 - 21. I 

30 33-3 75 20.8 

40 29.4 80 20.75 

SOLUBILITY OF LITHIUM CHLORIDE IN AQUEOUS SOLUTIONS 

op URBTHAN AT 25, 

fPalKuoh, l9S*fl. 19W.) 

to. Mola. per 1000 gas* HJ) Solid Ofo. Mol*. pfcr^lOOO tpa. H^O Solid 

..... ~~"" 



10.92 0,0 LiCl 22.40 9-2954 

19.93 0.2463 " ui.73 n8.336 
20.03 1.1528 " 

SOLUBILITY OF LITHIUM CHLORIDE IN ETHYL ALCOHOL AT DIFFERENT 

TEMPERATURES. (Turner and Biwett, 1913.) 
*' ^ms^OH 00 toMPto*. f. 

o 14 "42 UCUCaHsQH 20 24.28 LiCl 

5 15 -4 " 3 2 S- 10 " 

JQ 16.77 " 40 25.38 

15 18.79 " 50 24.40 " 

17 20.31 '* 60 23.46 " 

SOLUBILITY OF LITHIUM CKLORXDB IK MRTHYL ALCOHOL. 

(Lloyd, Brown, Olyn^n, Bonntl una jottti, ifPS.) 

Q OBS. UCl yr Solid 0i. LiCl pr SoXia 

C 100 *s. CH^OH PliMt l 100 



o 4^.3 LiCl.3CH,OH 30 n.8 

10 44. 2 LiCl (40 44. i 

1$ /m.O " $0 U4.4 

20 43.8 " 60 144.6 

SOLfTRILITY OF LlTHIfM CULORIOK IK ACETONK 

Powiiuia.'j, Samfura, TttMts and Jun@n, U50.) 



nuns. UCl par Solid (tat. UCl pur 

1 100 PIS. CHjCOCH^ Phftat C IQG pti. CHjCOCH.^ Fh*f 

o 1.73 LiCl 30 0.87 LiCl 

10 1.48 " 37 0,6l " 

18 0.95 " 40 0.69 " 

20 1.18 " $0 0.6l " 

The values at 18 and at 37 were calculated from specific con 
ductivity measurements by Lannuug, 1933. 



Li LITHIUM 



Cl 



SOLUBILITY OF LITHIUM CHLORIDE IK SEVERAL SOLVENTS, 

Cms, LiG Cms. Lin 



Solvent. *% Authority. Solvent. f. Pgo Authority. 
Solvent. Solvent, 
Alcohol: Alcohol: 
Methyl 25 42-36 (Tunw & Btoett, 19x3.) Amyl 25 9.03 (Turner & Bissett, 1913.) 
Ethyl 25 2 . 54* (Pattern IE Mott, X9<M-) ** ? 7- 2 (Andrews & Endc, 1895.) 
Propyl 25 16.22 (Turner & Binett, I9W-) " 25 g* (Pattern & Mott, 1907.) 
' r ? 15.86 (Schkmp, 1894.) Butyl 25 10.57* 





35 3.86* (Fatten fcMott, $904.) Glyccrol 2$ 4,3 


2* *< M 


Allyl 


25 4-38* " " Phenol 53 x.o, 


3* ** " 



Fused LiCI uwl 
ioo cc. anhydrous hydrazine dissolve 16 gms. LiCI at room temp. 

<WUb wad Bmitrwm, 1915,) 

SOLUBILITY OF LITHIUM CHLORIDE IN SEVERAL SOLVENTS, 

(Lasxciynski, tHi).;; ilcCuiuiuk, 1905.) 



2$ 



In Acetone, (L.) 

Gms. LiCI 

per ioo Gmii 

(CHa)sCO. 

4.60 

4.41 

4.II 



In Pyridine. <i..) IhGlycol. 



r, 
46 


Cms. LICI 
per too Gms. 
(CHWiCO. 

3-7^ 


r. 


(Jm. LICI 

t>er ioo Gnu 
UfiUN. 

7.78 


Gms. Lid 
* . Pr ioo Gms. 
SatSoL 
X S n 


S3 


3- 


IOO 


14.26 




58 


2.14 









SOLUBILITY OF LITHIUM CHLORIDE AT 25 IN MIXTURES OP: 



Acetone and Benzene. 
(Marden od Dover, 1917.) 



Gms, Acetone Gmi. UQ 

per 100 Gms, per 100 Gm. 

Solvent. Solvent. 

ioo 2.30 

GO 1.69 

80 0.066 

60 0.234 



Cms. Acetone 

r ioo Gn 

Sotvtnt. 

40 

ao 

10 

o 



^.,_. ,-,^^, Oms, LICI 
ptr ioo Omt. pr ioo Gnu. 
SolvtBt. 

0,088 
0,019 
0,OO9 



Ethyl Acetate and Benzene, 

(Murdten ami Dover, 1917.) 

Cm*. Ethyl Acrtalc Gms. LiCI 

pr too Gms. per ioo Gms 
Solvent. Solvent. 

ioo 1.78 

f* o,X47 

Bo 0,028 

70 0,005 



DISTRIBUTION OF LITHIUM CHLORIDK BETWEEN WATER AND AMYL 
ALCOHOL AT 30. 



U>hiir<u! I 



I : ) 



Mol.s L 


JQ per Liter. 


a. 
^ 

03.37 

04.1$ 

97.70 
ioa , 58 
110.40 


Mob. 


Lin pr Lifer, 


in. 66 
113.40 
117 

147,2 
216.66 


HjO lay^r M 
3-24 
3.06 

2-93 
2,82 
2.76 


,. Alcohol Layer t f . 
0.0347 
0.0325 
O.O3OO 
0.027$ 
0.0250 


a's 

2-34 
1.84 

0,65 


<i. Ak^hdl Layer f 

0,0275 
O,O2OO 
O,Of25 
O.OOJO 



SOLUBILITY OF LITHIUM CHLORIDE IN PYRIDIME. 



In Anhydrous Pyridine. 



B + 3%H,0 

by Volume, 



t*. 


urns. Ltu i 


wr too itnw. 


C^tllrf Ka* 




* Stt. Sol. 


Solvent, 


it*Uil I Mine, 


a 


n.3i 


12.71 


LiCLaCiH^N 


28 


11.87 


13-47 


14 


40 


u. 60 


13, 10 


Ll V * * CK$! A |^l 


60 


11,38 


I2.H4 


U 


so 


11.71 


13.27 


14 


IOO 


13.01 


14,98 


1C 



tr. temp, about a8* 



* > 


San, Sol 


halvent, 


32 


12,50 


14.31 


32 


*3-7Q 


15.98 


45 


$-5* 


18.46 


$3 


16,72 


2O.oB 


72 


17, 12 


20,66 


97 


8-35 


22.48 



9 i9 LITHIUM Li 

SOLUBILITY OF LITHIUM CHLORIDE IN QUINOLINE. 
(Walton and Wise, 1932.) 

Gms.LtClpoi- Solid ftnis. LtCI p<r Solid 

j." 100 gins. Quinolliw. Phase. t". loogmsQulnotlw. Phase. 

o ...... o.i5i5 (C 9 H 7 N),LiCl 56./S.... 1.1734 (G 9 II 7 N),LiCI 

. 2 5 ...... 0.3538 67 ...... i.a353 

^o ...... 0.6175 75 ...... 0.8180 

45 ...... i.o3a8 9(5 ...... 0.458K 

5o ...... 1.1107 

100 gms. sat. solution of lithium chloride in selenium oxychloride (So C1 2 ) 
contain 3.9.1 gms. Li Cl at 9,5. (\Vino, Ji-J3.) 

DISTRIBUTION OF LITHIUM CHLORIDE BETWEEN WATER AND AMYL ALCOHOL AT ^t4 0, 



The mixtures were shaken in sealed tubes of about 6po cc. capacity. One of 
these was charged 10 times, precisely similarly, and provided a total of 2.5 liters 
of the amyl alcohol layer. These 10 successive samples of non aqueous equilibrium 
phase were shaken in turn with one and the same small aqueous phase (100 ee.) 
in a second tube, and this latter analyzed for 01 by a silver titration method. The 
procedure consisted essentially in the piece-meal concentration of a large amount 
of the phase to be analyzed, and the concentration of the Li Cl dissolved therein 
by a piece-meal extraction of it with water. 

Om. inols. LI Cl per toot) gms. 
Anurox. Normality - ..... ............ ........... - * .......... * ............ -- - Partition 

of UOl Ir a<f. Phase. A({. phaso. Amyl alcohol phn*< cocfttt'tnit. 



o.o5 o.oSi o.oooi5'2 o.oo3o 

o.io 0.0996 o.ooo3n5 o.oo!)i!) 

o . 20 o . r 98 o . ooo(>6a o . oo3 ,1 5 

DISTRIBUTION OP LITHIUM CHLORIDE BETWEEN WA.TJBK ANI> AMYL ALCOHOL AT U(). 

(Uhtir, 192U r/.) 

Normality cone, of LI Cl In Norranlll} *umc. >f I.t (II i 

A<f. luy(r (C|). Atcohollo layer (C. t ). '0,* Aj. lttjft'{(! ( K A(c<ilioth 4 layer (<.' t i. <; a 

o.65 o.oo3o 216.7 '2.76 o.ou.Oo no.i 

1.86 o.oi25 147.51 tt-H* 0.0*75 ro'a,6 

tx . 3 4 o . 0220 117.0 v. . 93 o o3oo 97 . 7 

2.58 o . O2a5 1 1 3 . 4 "^ 0<) o - o3u5 c)4 , i 

2.68 o*oi4<> 111.7 3.'^i 0.0)17 93*1 

TOO gms. sat. solution of Li Cl in normal butyl alcohol contain u.jJu gms. Li (II 
at 9,3, and the density of the sat. solution IB d$:> 0.8713. 

' (Willttt'd aitd Smilli, IW*J, U2U rV 

Fusion-point data are given for the following systems: 

LiCl t KCl (Schauffer, 1919.* 

" * " * NaCl ( " f 

" NaCl (Schaeffer; Zemcznxny and Rimbach, 

" * LiOH (Scarpa, 1915. ) 

11 LiP (Botschwar, 1933.) 

11 * MgClp (Sandonnini, 1913, 

11 MnCl (Sandonnini and Scarpa r 1913. ) 

" NH NO (Perman and Harri.non, 19 24 a. ) 

11 + Pbfti ? 4 (Tries, 1914.) 

" * RbCl (Richards and Meldruro, 1917; Zmcznzny and Riwbach, 

1910; Keitel, 192$*) 

" + SrCl p (Sandonnini, 191 1, i^ua, 1914.) 

* - SnCl (Rax:k f 1914.) 

11 * T1C1 (Sandonnini, 



LITHIUM 

LITHIUM 



Gold CHLORIDE 



920 
LiAuCl, 



SOLUBILITY OF LITHIUM GOLD CHLOKIDI IN WATER. 

IBM.) 



100 



Solution 



10 53.1 40 

20 57-7 50 
30 62.5 

LITHIUM CHLORATE LiClO, 



Cta. LIAuCl ptr 
100 Cto* Solution 

67.3 
72 



100 



60 

70 

80 



L1AUC1 4 per 
feu. Solution 

76. n 
85.7 



SOLUBILITY or LITHIUM CHLORATE IN WATIK. 

(Krau ones Burgtjst, t9F7.) 

The determinations were made by observing the temperature at which 
the last crystal of solid phase disappeared in the melt. Careful control 
of the temperature and vigerous stirring were necessary. The mixtures 
were kept under a slight excess pressure or dry nitrogen. The tempera- 
tures were read by weans of a copper-con 3 t an i<m thermocouple. 



.0 


Ctos. LiClO,., pur 


t 


100 0R* Mt. Ml. 


-8,7 


15.76 1 


-13.2 


20,73 


""17*4 


24.44 


-23.3 


28.68 


""30.5 


32.71 


-36.6 


3508 


"40 . 


37.00 


"37-1 


38.10 I 


-33.9 


39.05 


"15-7 


45*35 


-8.8 


47.94 


-4.8 


50*49 


-1.8 


51.95 


+ 2.2 


54.57 


4.8 


56.6l5 


6.) 


58,16 


7.3 


60.15 


8.0 


ro.pl. 62.60 


7.9 


63-44 


7.4 


64.88 


6.0 


67*18 


3.4 


69.74 


"*"! *S 


Ru tec. 7 1.1 


-1.7 


72.59* 


-3.6 


73*74* 


-7.6 


75.15* 


-9.0 


Eutec.75.7* 


-13.6 


77.25* 


-25.0 


Bu tec. 81.0 



Solid 

Phase 



(Ms. 
100 P 



pr 
. toi. 



Ice 



LiCl0 



3.8 


71.89 


6o 


73.60 


9. i 


73-74 


la.o 


76,08 


18,9 


78-54 


ai.o tr.pt. 


81.2 


,0*1.3 


76,59" 


+ 3.0 


77-59* 


8.4 


78,13* 


12. & 


79.26* 


16.4 


79.68* 


22.1 


81.68 


37.4 


83*17 


36^5 


84.94 


41. s tr.pi. 


86,6 


36.9 


66,37* 


43*9 


87.17* 


48*7 


87.0 


64.4 


88.81 


71,9 


90,35 


86 3 


93.45 


^95*7 


94. OS 


90*0 tr.pt. 


94.9 


103*0 


9S08 


115*2 


97.43 


133.0 


98.86 


137*3 n.pi. 


100.00 



Li CIO, 



LiOlO, 



V 



yucio. 



"flCUCKX, 



( LiClO- 



The previous determination of Hylius and Funk, 1897 i8 is much 
below, and that of Carlson, 1910, is considerably above the present 
results. 

Additional results agreeing with the above Are gives by Berg t 1929. 
This author gives evidence that the y modi fi cut ion of LiCiO is really 
the hydrate aLiClO^.H^O, the existMce of which he reported i a 192 6. 



921 

LITHIUM Per CHLORATE LiClO^H 



LITHIUM Li 



SOLUBILITY OF LITHIUM PERCHLOKATI IN WATEJU 

(Simons and R09P 19P8.) 



d. of 
sat. sol. 100 0s. a c 






1.215 


10 


1.236 


20 


1.258 


25 


1.269 


3 


1.277 


40 


1.300 


64.6 





77*9 





89.2 





92.3 


- 


94. 3 


"-"" 


95.1 


m.pt. 


94.8 





93-2 


- 


92.7 






29.90 

32.88 
35*95 
37.48 
38.87 
41.97 
50-, o 

60.0 

62.5 

65*0 

66.32 

66.67 

70.00 
70,3 



Solid 

sol. Phut 

11010^3^ 



OM. L1CJLO, 



Soli a 



jU9253 


70*33 


93.2 


70. S 


97.3 


71.0 


108.9 


72.8 


120.7 


75*0 


136.9 


80.0 


144-0 


82.5 


1^8.5 


85.0 


149.0 m.pt. 


86,5 


149.1 


87*S 


14*1.2 


90.0 


145. 7S tf.pt 


. . 


167.5 


91.04 


172.0 


91. 11 


236.0 mpt. 


100.00 



IOC . Ml. Ml. HllMKft 



LiCIO 



LiClfV 



LITHIUM Per CHLORATE Li CI () 4 .3If t (). 



SOLUBILITY OF ANHYDROUS LITHIUM 
SOLVENTH AT 25. 



PKRCHLORATB IN 
( Willard and Smith, 



LiClO, 



WATER AND IN 



CIO 



Solvent. </ of iMilvrut. ,/ f nut, M>|, 

Water 

Methyl alcohol 0.78705 

Ethyl alcohol 0.78517 ,3173 

n Propvl alcohol o . 7989 , '1,006 

n Butyl alcohol , o . 8069 . i HuO 

i$o Butyl alcohol, 0.7981 

Acetone , . . o . 785^ 

Ethyl acetate. 0.89(57 

Ethyl ether 0.70817 

SOLUBILITY OF LITHIUM PBRCHLORATB TRIHYDRATK IN 

( Willard and Smith, lUW. \ 
</of GmN. UIO ptsr 



.at. Mil 



Solvent. Kat. itol. 

Methyl alcohol. , . i . i/jao 

Ethyl alcohol. ... i.ouji 

n Propyi alcohol. 0.9349 

n Butyl alcohol.. 0.908'! 



It. HOt, 



(10.95 isa Butyl alcohol. 

4a.i6 Aeeiora*;,.. i. 

i6.8'>. Hthyl 

21.40 Kihvl 



67. 7 

4B,7 f 
VI :n 

8oi,VNTH \T ' 



.8887 



tw m tnt 
I8.H5 
49.04 



SOLUBILITY OF LITHIUM PRRCHLOAATK THIIIYDIIATK IN MIXTUKXII 

OF ETHYL ALCOHOL AND ETHYL ACETATE AT ^5, (Smith, ia,.j 



Vol. percent C,Il ft 
In solvci^. 

o.o(=CH coQc a ng. 

10. 

20.0 



ftnifi. J 

per 100 fnis. MSI, 

'>,(* , 3 > 



Vol. 



., Oil 



. 1414 (I, 



33,59 

3o.o 35.10 

4o.o 3(5.5! 

5o.o. ^^ 



lit soivrul 


pir iflM . * 


60 . o ....... 
70.0. ,...,. 


;j-^ 


80.0. , . . . . 


/ uV 


90.0. ,.,,. 


. . . . . 4 1 ~i 


IOO.O. ...... 


...... 4* , y / 

...... ^'i.!( 



Li LITHIUM Q22 YY/ ^ 

LITHIUM BICHROMATE Li a Cr a O,.2H a O. 

SOLUBILITY IN WATER AT 30. 

(Schreinemaker Z. phyaik. Chem. SS 79. '06; at sS, Mylius and Funk Ber. 30, 1718/97.) 

Composition in Wright per cent: 

Solid 
I'hase. 

LiOH.HaO 



LiOHJIjO 4 



CrO 



Of Solution. 
%Crt) 3 . %UiO. %C 


Of Residue. 

:rOjj. %UaO. 





.0 


7 


'09 










6 


.986 


7 


744 


4. 


322 


18 


.538 


16 


.564 


8 


.888 


10. 


089 


19 


SS^ 


2 5 


.Sir 


10 


.611 


15- 


479 


21 


. 1 06 


33 


.618 


12 


.886 




365 


X9 


-398 


37 


.411 


14 


.306 


44. 


S55 


17 


.411 


37 


.588 


14 


.381 


36. 


33' 


18 


552 


37 


495 


13 




5*- 


075 


16 


.384 


40 


.280 


10 


^858 


, 








43.404 


II 


,809 


S3' 


703 


14 


.070 


4S 


.130 


9 


5^5 


5<>. 


085 


10 


. 190 


47 


945 


7 


95 * 


S- 


029 


9 


.238 


57 


.031 


6 


.432 


6S- 


560 


a 


733 






S 


7*3 


7i 


687 


8 


S'J 


67 


.814 


S 


,689 


80.452 3.780 


65 


.200 


4 


.661 












2 57 


2 


.141 


85'- 


914 


o 


-758 



aH a O + CrQi 



CrOi 



62.28 



A saturated aqueous solution contains: 

49.985 per cent Li,CrO 4 , or 100 grams ILO dissolve GQ.Q* s y rams 
Li,CrO 4 at 30 (S.). 

56.6 per cent Li,Cr 9 Tl or 100 graniH ILO dissolvo 1^0,4 irrams 
Li,Cr.0 7 at 30 (S.). 

52.6 per cent Li 3 CrO 4> or too grams ILO dissolve no.o rams 
LiCr0 4 at x8 (M. and P.). 

Sp. Gr. of sat solution at x8 * 1.574. 
LITHIUM FtUORIOB LiP 

SoL0BiLiTir or LrrxxoTN PLUCK IDS in WATIK. 




18 

25 

25 

25 

35 



a. &t 

3&U 301. 



0.99811 
0.9958 



ur 



100 



H ? 



0* 130 

0.27 

o* 151 

0. 113 
0. 1 33 
0-135 



I My it us 4nti Funk, 1897 
1 Carter, ig aR. I 

and Dwukei, 1931, ) 



Solubility of Lithium Fluoride in Liquid Hydrofluoric Ac id. Determina- 
tions of the Solubility of LiP in liquid HP by toiul and Siowe, 1931, 
show that the reaction LiP * HP " LiHP f occurs utd the molecular ratio 
LiF ; HP in the saturated solution at tennperAtureu betwuen o and 40, 
is approximately 0,043. This corresponds to 5*59 gma. LiP per 100 gms. 
IIP. Predenhagen and Cadenbach, 19*50, 1931, 19:11* found that a. 6 gms, 
LiP dissolve per IDOCC sat. solution of LiP in liquid HP At 18. 



923 LITHIUM LJ 

looo gms. pure Acetone (CH,COCIL) dissolve 0.0000033 i**- LiF at l8 
and 0.000004 gnu at 3 7, as 3etermined by conductivity measurements. 
iu u.vu ^ (lannung, 1932.) 

Fusion-point data are given for LiF + LiOH and Lil * LiOH by Scarpa, 
19 i S and for LiF * MgFj,, by Tacchini, 1924. 

LITHIUM Titanium F"LUORIDE Li g TiF fl . aH^O. 

SOLUBILITY IN WATBH AKD iw ETHYL ALCOHOL AT 20-22* 

(Oinsbtrg, 1032.) 

1 
lOOcc Solvent So Ho Ph&ae 

Water about 56 Ll fT? F 4:^ 

48 



98% C p H 5 OK 0.035 Li 



f 



0.030 
LITHIUM OERMANATE 3 LiGe0 3 Jl ? 0. 

100 gms. sat. solution of Lithium Germanate in Water contain 0.8*1 
gnu LiGe0 3 at 25. (high, 1926.) 
LITHIUM IODIDE Lil-aHA 

SOLUBILITY IN WATER. 

(Krcmcrs, 1858, 1860; ice curve, Jonen, 1907 ) 

Gms.perxooGm8 ^^ C^MWI^IH. 

Water. Sat. Sol. Water. v "' i "' 1 



0.296 i. 08 i. 06 Ice 20 165 62.2 

1.218 4.36 4-19 " 2 S x ^7 62.6 

2.70 8.71 8.02 " 30 171 63.1 
- 6.14 17.69 15.03 " 40 179 64.2 
16.2 38.31 27.70 " 50 187 6|.2 

25 48.67 32.72 " 60 202 66., Q 
-SO 85.13 46 " 70 2^0 69.7 
6q Eutec. 03 48.2 Icc+UI^HjO 75 263 72.5 
~6o loo 50 LiLpHtO 75 m. pt, 

40 118 54-13 % m. pt. 

-20 134 57.27 " 80 435 81.3 LiLHaO 

o 151 60.2 " 100 481 82,8 4< 

to 157 6i.x " 120 590 85.5 ** 

A more recent determination of the Butectic point for Ice * LU . 3iI f O 

by Huttig and Steudemann, 1927, is -91 and 107 gms. Lil per 100 gms. H f O. 
SOLUUIUTY ov LITHIUM IODIUIS; IN 
id Pohlc, am, ) 



Gms. 1,11 
t 1 *. per 100 KIU.S. < 

f ^ T 


D. Solid 1'hatit;. 

LiL3H 2 





w-HLil.^HaO. 
Lil.iHtO 


t" pr 

77. . . . 


I'HI gm^*, ti,0. Holht I'ha.r 

4^7 Uriul^O-*. Lil.I: 
413 LiI.tH,0 

437 

W 

743 
787 
BuO i hi!, 
83"> IJIJ/,!!,** 


IQ 


179 
200 

286 

*97 
3o6 

372 


80...., 

88 


AO 4 * . 


5o 


99 


% 


rjo 


71.5.... 
70.5.... 
71.5.... 
7Q 


i3!!!!! 



The authors also give vapor pressures and thermo chemical datn. 
100 gms. sat. sol. of LiI.3H f O in Water contain 61.2 gw. Lil at ig. 

(LaanuAg* 19 
100 gms. sat. sol. of Lil.3f .0 i n Water contain 61.6 ems, Lil At 



Li LITHIUM 

LITHIUM IODIDK 

EQUILIBRIUM IN THI SYSTEM LITHIUM IODIDI, 
IODIDI AMD WATER AT 25. 

(ng>@alux ana Roger, 1937.) 

The results are given in the form of a diagram but the experimental 
determinations are not reported in the present paper. The following 

approximate values were estimated from the diagrams. 



Solla 



d. of 


QMS. ptr 100 tjaa- 


Soiia a. of 


ftaa. 


per 100 gM. 


sec. sol. 


aau 


solution 


PH&s* & sol. 


Mt 


* iwluuon 




,_ 


u! ' 




'Wj 


Lil 1 


1*815 


0.0 


62.2 L 


11,3^0 2.160 


28.0 


40.5 


1.885 


5-0 


55-8 


" 2.195 


31.9 


1 3$. 53 


1.970 


10.0 


55'^ 


M 3.140 


30,0 


38.0 


2.080 


16.0 


53*5 


" 1.840 


22. S 


37.0 


2.l6o 


21.5 


50.0 


"+ 1.1-41.590 


*5*Q 


35*0 


2.135 


24.0 


45*0 


1,1.4 1.350 


5.5 


31.0 








1.330 


2.0 


25,0 



Pbl. 



= Lil.Pbl 



? ^ 



EQUILIBRIUM IN THR SysttK LITHIOM IOIIE, AHTIMONY 
AND VATRH. 

wui ru-lwfiuUo, 1930.) 



The results 


are given 


only in the form of a di^ri 


from which the 


following approximate values were read. 


Results 


at 13 


Resu 1 1 s 


at H 




Results 


at 60 


OBis. per 100 


jVV 


fton. por IM 


M. *vo 


Qna* pr 


m pi* H^O Solid Phaoe 


' * r 


^^ 


3 


' til ^ 


Sbl^ 


~ rrr ' 


^ it each Leap, 





160 





1^5 





. 9S 


LII.3H.O 


So 


162 


50 


176 


so 


196 


H * 


75 


!3 


105 


176 




305 


"* 1.1.6 


65 


130 


9S 


ISO 


125 


i8s 


1.1.6 


55 


no 


85 


120 


1 15 


155 


M 


70 


80 


95 


100 


135 


135 





8s 


so 


80 


$30 


150 




M 



1.1.6 = Lil.* 



DlSfRlBWTIOK OF LlTWXtJM TOOXDI 
NXTXOBIIUINB AT 



WATIR 



O laytr 

4*55 
2*38 
1.57 



fr nur 



0*OOUO 



0.00363 
O.OOiq* 



H t> 
3350 



925 LITHIUM Li 

SOLUBILITY OF LITHIUM IODIDE IN SEVERAL SOLVENTS. 



Solvent. 


t G s< Li J \ t Authority. 
* xoo dim. Solvent, 


Methyl Alcohol 


25 


343-4 


(1'urner and Bissett, 1983.) 


Ethyl Alcohol 


25 


250.8 


" 


Propyi Alcohol 


25 


47-52* 


iii ** 


Amyl Alcohol 


25 


112.5 





Glycol 


15-3 


38-9 


(de Coninck, 1005.) 


Furfurol 


25 


45 -9t 


(Walden, 1906.) 


Nitromethane 


O 


I .22| 




(i 


25 


2 .52 


i 


* Solid phase 


LiL4Cyr 7 OH. 


f - gms. i>er 100 cc. sat. solution. 



loo gms. pure Acetone (CH^COCH, ) dissolve 42. $6 gms. Lil at 18 Md 
75.25 g"s. at 37 as detennxned by electrical conductivity, flaunting, 

S933.) 

F.-pt. data for Lil + Agl arc given by Sandonnini and Scarpa, 1913. 

LITHIUM IODOMEBCURATE 2LiI.HgIi.6HjO. 

TOO gms. sat. solution of lithium iodomcrcurate in water prejMired by cooling a 
hot solution and allowing to stand at 24.7 for 3 months, contained 1.30 I(WH, Li, 
27.4 gms. Hg, 58 gms. I and 13.3 gms. Hat); Sp. Or. of the sat. sol. 3,28. 

(I)uMn, 190$.) 



LITHIUM IODATE Li(lO,).iHjQ. 

zoo gms. H a O dissolve 80.3 gms. LiI0 3 at 18, or 100 gms. solution contain 
44.6 grams. Sp. gr. of sol. 1.568. (Myl!u ad Funk, x%7.) 



LITfflUM PERMANGANATE LiMn0 4 .3HiO 

loo gms. water dissolve 71.4 gms. permanganate at 16. 



LITHIUM MOLYBDATK ^Li Mo0 4 , 3H ? 0. 

SOLUBILITY op LITHIUM MOLYBDATI IN WATI*. 

m ana Retjlln, ],9?U) 



per tOO 0ns. anc. aol. PhM@ l pr 100 *t 

o /is- 2(4 if!a 8 Mo0 4 .3H 30 44. a6 |U t Mo0 4 .3H R 

20 ^4.30 " 40 43.84 " 

2 S 44.8l " 98 42. <0 '* 

The result at 20 is by Wempe, 191.1. 

Fusion-point data for mixtures of Li MoO * ffoC)^ ^ui LiMoO * NA MoC) 

are given by Hoermann, 1929. * 4 



Li LITHIUM 926 

LITHIUM NITRIDE LiN 5 .H f O. 

SouttiiiTY or LITHIUM NXTIZDX IK 



tea. UN. ptr 
f o ^ 

ICO pi* ai. Mi* 



, pr 

b Ml. 



-10 

-30 



10*0 Jce 

30.0 " 



38,0 



i|0.0 



LiN v ilLO 



uo 



UN. 



The results in the iMiIf, ^xc^|*i ihuse tor the euttciic and 

the tr.pu-, were tfii4ttI 4|>nrPiAiely frtw ihe A!hors diAgran. 
The preceding renuLm of Curust* Ad RUww, ioH, ^re considered to 
be in error except the value for 16 which fairly well with 

the above. 



NO 



NITEIT1 LtNC)i.HA 

Y IN WATRK. ((Hw*w, tit) 



Grot, 

UNOi per 
100 Groi. 

Sat. Sol, 

11. 1 



t\ 

xi, 7 15 

21 21.2 
-28.8 29 
-31.3 29,4 

o 41.5 

+ 19 48C 
25 



let 



M 



. i#rr 



4J 



$ft 



40.$ ^ * 

6$ 6 1 H 

81.5 6H.7 

Qt 71 4 

96 g t H 

03. S 04 ,1 



Solid Ihas, 



ioogms.HiOdiMolve 10.5 gtn* AgNOt ^ girw. LiXOiiit 14*. (Ckwaki, 1914.) 



Recent deieriaitiofis of ih* S^iubtluy of liihtu 1 * Nuriie by Bureau, 
ht following rf%!ti 4if faring fr*** ^** above. 



ptr 



Soili 



tOO IM. Mb 

- f|9 7.01 
-10,25 13,11 
-24.25 31. 08 

-38.7 Bu tec ,36. 58 

^3.7 139 

-10*05 40,5 

* 79S ^1*S 



let 



lB.ii 



66.0 







'I5 



1*113 



*6.6 LlNO f .H f O 



61,0 -*UW 

63 < 

66.4 

70.2 



LiNO f 



76, LiNO f 



Solid 



Q27 LITHIUM Li 

LITHIUM NITRATE LiN0 3 .3H 2 O. 

SOLUBILITY IN WATER. (Donmm and Burt, 1903.) 

Gms. LiNOa 

Solid Phase. 4. per 100 Gms. 

Solution. 

LiNO 3 ,3H 2 29.87 5^.42 

29.86 56.68 ** 

" 29.64 57.48 " 

" 2 9-55 58.03 " 

" 43.6 60.8 LiNOa. JHiO 

50.5 61.3 " 

" 55 #3 

" 60 63.6 

" 64.2 64.9 LiNOa. 

70.9 66.1 

The eutectic Ice 4- LiNOa-sIM), Is at -17.8 and about 33 gms. LiNOj per 
loo gms. sat. sol. Transition points, 29.6 and 61.1. 

Data for the system LiNOa -hLigSOi+HaO a t o, 30 and 70 are given by 
Massink, 1016. 
EQUILIBRIUM IN THE SYSTKM LITHIUM NITRATE, LITHIUM SULPATK AND WATKII 

AT 25 AND AT i5. (MuKHillk, HUH.) 





Gms. LiNO,T 


t 


per 100 Gms. 




Solution. 


O.I 


34-8 


10.5 


37-9 


12. I 


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 



GUIS, ptM* too gius. 
sat. sol. 

UNO;,. M 8 SO,. Solid J'liHHo. 

llcsuks at 2. r ). 

47.58 0.0 LINO a .:iH a O 


(an. (id* ion HUH. 
siil. sol, 

UNO,. 1,1,80,. 


8: 


Go 
45 


dro 

0, 


>n-M a so,.H( 57 

,19 MgSOi.lM) 5 a 


'.o3 


'ho. o 
'.' ;o. o 


33. 


9 


i . 


!^ *> 


.)() 


,55 


1 :o.< 


0. 





8 


./M 

79 


t, 


.5/5 


o oS 
0.17 


Results at 35". aK.(>3 




5o. 


4g 


o 


.0 l-INO.t.'/jHuO 


2'.i 


.|H 


5 . 1 f > 


o'i! 


9* 


o 


.0 UNO;, 


20 


.'4 


<i. 7 8 


61. 


97 





,o >H-I.I80t 






M.I 



SolUl IMa', 
UNO, t'UljSO, 



M.lt. HOI, 

M NO.,. I.I, SO,. Htilht t'JM%', 



^.,4K 

^ jr , i 

^.i.HH 

a,j',^ 



..48 



' 

SOLUBILITY OF LITHIUM NITHATU IN AQUBOUS Sotuxiows op 
LEAD NITRATE AT 25 AH VICK 



QMS, per 100 g^a. sat, sol, 

, __. __._ 



43.83 



33.96 
29.15 
28.36 



Ons. ptr tOO tj^i* sat. aol, 

r ^^^ 



o.o 

2./I7 

2.6$ 

5.10 Pb(NO s ) p 

6,30 " 

8.6s 



21,54 

10.88 
0,97 

0.57 
0.0 



9.3^ 
*sso 

3130 
11.12 
37.07 



EQUILIBRIUM IN THE SYSTEM LITHIUM NITHATI, TITIAY BUTYL 
AJLCOHOL AND WATER AT 25. 

(Qlnnlnga, Hftrnng ana wobb, ia;n?,.i 

The composition of the homogeneous mixture (plait poiat) of the three 
compounds as determined by the synthetic method is 16.0 gws. LINO. + 
23.0 gms. tertiary Butyl Alcohol, (CHj{jCOff t per 100 gms. s&i. solution. 
The original results for the remaining points on the biaod&l curvt Are 
not given but only the values corresponding to derived empirical 
tions for the curve. 



Li LITHIUM 



LITHIUM NITRATK 



SOLUBILITY or LITHIMM MTRATI in Uytun VWONIA. WRTRRMINK& 
BY mi SYMTtiiTic MRTHOI*. 



QM. UNO,, 



-77.7 
-77.8 
-79.0 

-78! 5 
-62.0 
-53.0 



o,o NHj -jrfi.* 

^03 M -li.o 

10.71 " * ^ 

21.71 " * *' 

24.26 Li. 8 - .o 

33 Si / *'S 



111! 



>o.o Li NO 

(70.80! M ' 

** I *? (t 

7rf. ,s " 



lHi,f 



Li. 8 = LiNO^.BNI^; li,i - l.iN' ? .aM%; i-t . .* - i.i^i f ,j,in n,i diuhors 
also give results far itii* iJenuiiif.* of :4Dhitu(tH of ItVu^.in Hll^ 41 30* 
The results HI a$ e in p,irf*nth**sis ,ib*w 



Hiiuf 



NO 



SOLUBILITY or LITHIUM NITHATI i* 



u iw. 

HY THE 



>#r. 



Hoi. ftrctnt StolU 



16.6 o.o CII^CIIOH ijt,< * 

16.3 0,156 ' " t.Hi "i. 

16.03 09R3 ** IlU*)J 111. 

15.71 a. on " 1*1*0 *^ 

15.0 4. us ** ^. i 

ii), i(6 5*305 M ^*j 



* MetastAblf 

A saturated aointicift of Itifiiiw 
mols. = 23.67 g. LiNf) 3 pir liter 
Lewis, i^tul 



U 



JtNH, 



!** tn At*ii*fl** 



Solid 

Phui 



I7.o8 
10. 8ft 



SOLUBILITY OF Litmt.'M NHHAH-. i^ ,Stitiu ^MI% 

*. H- I ^ Ml, ! 

HwSirnS ' 

Aeetottitrilc, ..,,,,..,,,, , . 

Fso iriiy! atrotiof. ...,...,,... ** , \ i 



i-, ii , it*j,i 



929 LITHIUM Li 

EQUILIBRIUM IN THE SYSTEM LITHIUM NITRATE AND UREA. 



fltas. UNO S Pr SoliU OBIS. L1NO^ per itolld y Ores. LINO, pr itolld 

100 ipns. Mixture Phase toe Es. Mixture Pft&se ^ 100 PQ Hi x lure Hianf 



132.0 


0.0 


COINH,) 71.0 


18.8 Co 


{NH^+i ,21,^.7 


,v>. v) 


126.7 


2.78 


64.1 


19.83* 


" 132<O 


42. 2S 


122.3 


4-67 


" 44 7 


22.98* 


" 1 1 'U 2 


46 . 16 


113-9 


7. .93 


" 1 06 . 8 


25.68 


1.2 i on . i 


48.6-i 


los.o 


10.79 


113.5 


27.89 


" 100.6 


50. j8 


102.9 


11.31 


117.5 


29.;6 


98,5 


;o.oo 


90.1 


14.53 


" 122-5 


32.6 


121.1 


U>,8s 


74.0 


19-52 


" 1 25 - 9 


35.92 


11 M7'J 


54. o 










146.4 


57.07 



* Metastable, 1.3 - LiN0 3 , 2 CO(NH 2 ) p . 

Fusion-point data are given for: 
LiNO ? Li SO^ (Amadori, 1913.) 

" " + NaNO (Oarveth, 1898; Lehrman *md Breslow, 

" + RbNO^ (Puschin ami Radoicic, 1937.) 

" -f TlNO^ (ftriscoe, F<van5, and Hobinson, 1912*) 

LITHIUM OXIDE U ? 

Fusion-point data for the System Li f O * V^0 ft are* given by C!4Ui*n , jgjM. 
LITHIUM HYDROXIDE LiOHJ!/). 

SOLUBILITY IN WATKR. OH 

(Diltmar, iHBH; I'jckeririK, IKM.) 

Gms. per 100 Gms. C ; m>it Li( ,j j 
Sol " tlon .- IHT ioo (irns. 



-10.5 


LW> - 


LiOH. " 

7- 2 3 


Hs.0. 


30 


7,05 


,. , i * ' ' ' * 
l,u|i " I! n 

H ,y i.'.g 


1 8 Kutt-c. . . . 


11. 2 




40 


7 . .?ij 


I 1 . <K i ^ 





6.67 


10.64 


12.7 


50 


7.56 


i.?. i . i i ^ 


10 


6.74 


IO . 80 


12.7 


()O 


7 . t)^ 


l .! . yO 1 -; ,S 


20 


6.86 


I O . ()() 


12.8 


80 


K.Hy 


14. ,'l H A 


25 


6-95 


II .14 


I 2 . C) 


IOO 


I O , O2 


1*1.05 17.5 



o ioo gms. sat. solution of LiOil.|| p O in Water contain 10.7 ^HIM, ttdfl 41 
o ; (Rollet and Lauffenburgcr, i^in*); u,i^ urns, ,u as 11 iV.yi Mfiir., 
1916); 11.0 gms. at 25 (ifeda, 



SOLUBILITY OF LITHIUM MYDKOXIDK IN Ayi/Kot's SdLt^ntJNs ut- I mui M 

SULFOANTLMONATK AT 30" AM) VlCK V'KKSA. 

(Donk, iyo.) 
Gms. per ioo Gms. <;,, fK , r |OO C;TO ^ 

bat. Sol. Solid Phase. _liL, So1 J .,,!,,! ft, t *. 

LiOH. Li 8 SbS t . LjOH, "^7^7 

I3C -4 O UOH.H,0 2.1 48.3 Z,,OH!M> 

^' T S '3 " 2.1 52. i " i |.,.M,*; <IO ||. 

2 '3 29.9 - !, 4 ^ fK l^ShSnj^i 

O c r , i 



Li LITHIUM 930 

FntllLIBRIUM IN THE SYSTEM LlTKIUM IlYDIlOXUH-:, Plir.NOl. AM) \V\TE 
Cl< u | Vuu M*urs, itlili j. 



-EH M ajjo 



Mols. per 10ft moli.. 
sut. sol. 

^.79 o.*o ' Li OH. 11,0 

8.3o o.23 ^ ^ 

S'.'S uo-1 riH,OW. ; *H^'> 

2.64 '2-37 ** 

n 3.a5 7.7* * 

OH 3.79 i<-38 

4.28 22.64 



I.tOH, 

4, -in 



1.08 (18.71 

'l.H 7K/}' 

1.14 7>->i 
;,.i. u 



4.28 22.64 '* : UH^OH 

At concentrations of Li OH b*low o.iS mol. per wit, liquid kyttrs with 
following composition are formed. 



the 





PO 



LITHIUM PHOSPHATES 

100 gms. sat. solution of aeuirai Lithium 



in water contain 



0.022 gfl. ^^3^4 t Q ACt 0.0 3O g * I 30, 

100 gns. sat. solution of *cil lithium plio.-ipH.iie in water contaia 
55,8 gms, LiII g P0 4 at o fRoUtt mil LftuffenUurger, 191.^ 

IK THi SYST1W LlTHXUN OlXDX, POSF0WS 

PtKToxxot AKO 



Results at o 

toa. per 100 BoUd tat. 
pa. sat, aol. Ptiaaa p* 


i^-r 160 

Mt. i9i. 


Kr.Huitn at 30 

ioUa nnf. ;-es too ttolia 


0.0 


Li 

6. 


71 LiOHJI.O a. 


1 
7*4 


0. 


74 


U,PO o?,,i, 


7. 


os LiOH.H f O * Li 8 P0 4 


0.015 


6. 


72 H 


4 V 


PO 11. 


0^ 


3. 


55 


" 0.0165 


C>* 


077 l'*jiP0 4 


0. 


02 


S 


58 Li, 


.PO ' 


17. 


2 


1* 


90 


" 0*0310 


Cl 


fl I ^tt ** 


0* 


Ol6 


2. 


IjO 


M 


20* 


a6 


4* 


58 


** O.OJ7J 


0* 


16 5 * 


0. 


02 


0. 


'19 


tt 


aa* 


16 


4* 


47 


0.035 


0. 


0107 w 


0. 


0148 


0. 


0088 


H 


2H 


10 


1* 


43 


w oo 160 


0. 


0301 H 


0. 


Ol63 


0. 


0098 


tt 


1* , 


11 


6. 


86 


0.nS 


0. 


5^ " 


0, 


0375 


0. 


0185 


H 


34. 


3 


7* 


55 


11 o.aaa 


0, 


C^6S " 


0. 


058 


0. 


025 


W 


37. 


9$ 


8. 


19 


Llll f ro 4 0.305 


o* 


lift 


0. 


388 


0. 


X49 





38.10 


8. 


oB 


w 0*H09 


0* 


HO ** 


0. 


414 


0. 


167 


H 


18. 


20 


7. 


68 


** o6 


0. 


ao$ H 


0, 


452 


0. 


174 


H 


38* 


45 


7. 


S4 


** 0*871 


0, 


a6a " 


0. 


635 


0. 


2285 


W 


18. 


83 


7* 




w a? * f 


v 


71 


0.782 


0. 


266 


H 


47- 


5 


4 


,6j 


^ 17.1 


7. 


6"i w 


0*80 
0.96 


0, 
0, 


.270 
>33 


H 


55 1 


6s 


a! 


,74 


" Kk6 


a! 


!^ lf * LiH f P0 4 


1. 


355 


0, 


403 


H 


ssls" 


3* 


.23 


" HU7 


7. 


.7-j LiH P0 4 


1,88 


0, 


,520 


H 










41*5 


6. 


6 a 



93 i 



LITHIUM Li 



LITHIUM PHOSPHATE Li^PO,. 

Aqueous solutions of lithium phosphate are colloidal and cannot be obtained 
clear. A solubility determination made by electrolytic conductivity gave 
0.297 gm. Li 3 P0 4 per liter sat. solution at 9,5. /Hosenlunm and Iioglw, mu 

LITHIUM Sub PHOSPHATE Li 2 l > O; i .3/sH, t O. 

100 gms. sat. solution of lithium subphosphate in water contain 0.1018 gm. Li t PO 8 
at o, o.o575 gm. at ^5 and o.o4# gni. at /jo . These determinations are only 
approximately correct since it was impossible to obtain the saturated solution tu 
a clear condition either by long standing or by filtration. A determination made 
by electrolytic conductivity gave 0.1267 gm. Lig POg per liter sat. sol. in water 
at 25. (IloscnUcitn and Urj^lin, Itttl.l 

LITHIUM Hydrogen PHOSPHITE Li s H PO a .H 2 0. 

SOLUBILITY OF LITHIUM HYDROGEN PHOSPHITK IN WATJK. (aoonhim a*<l iieglin, HW.) 

Cms. LlgHPOi per (Jm*. I,l,IUO a JM-C 

100 gms. sal. sol. Solid Phase. t". )<>0 gmt. sal. ol. SiiUd I'tinNi*. 

.., 9.07 LIAWO^O 4-, ti.wj Li l HPO a H,U 



PO 



t". 

o 
25 
3o, 
35 



7-<>7 
(>.8->. 



LITHIUM (Hypo) PHOSP3BATE LuPiO.7H0. 

100 gms. H 2 dissolve 0.83 gm. hypophosphate at Brd. temp. OUmmdibax, 



LITHIUM SULFIDE Li g S 

Fusion-point data are given for li f S t S by Pemrson and Hobinson, 
LITHIUM Antimony SULFIDE Li-SbS.-ioH.O. 

O 4 I! 

SOLUBILITY OF LITHIUM AWTXMOHY SULFIDI in WATEI ANS IK AQQIOOS ALCOIOL 

In Aqueous Alcohol at 10* and 30*. 

Gmn. per 100 Gms. 



In Water. (Donk, x0o8.) 




Gms. Li s SbS< 




t a . 


per xoo Gms. 
Sat. Sol. 


Solid Phase. 


- 1.7 


7.1 


Ice 


- 3.2 


12.8 




5.1 


I7.S 




-10.8 


23,2 




-xs.9 


28.* 




26.2 


35-3 




-42 


40 . 4 lo 


t-fLiiSbS^.toH 




+xo 


46.9 


Li,SbS 4 .xoH 8 O 


30 


So. I 


M 


50 


51.3 


*4 



Sat. Sol. 





10 
10 

30 
30 
30 
30 
30 
30 
30 
30 



10,7 

26,2 
66,2 



54.8 

5-4 

SS.6 

65,26 

74-3 

79-S 



41.3 
36 5 

20,6 

46.3 
30.7 

30.8 



24-X 
30,5 



Solid Pbai*. Authority* 

LlsSbS 4 ,io^O (Donk, 1908,} 



(Schrtta* 



1910.) 



i LITHIUM 

LITHIUM SULFATE 



SOLUBILITY or LITHIUM Star ATI IN WATER. 



-16. 

-13- 
-11. 

- 6, 
o, 
o. 

0, 

16, 

25 
25 
31. 

(1) 
The 



8 



Own. U ? SQ 4 ptr 

100 EW* M ^* M *" 

27v 

37 44 
27.1H 

26.73 

25.43 t 

26.31 ? 2* 

26.<1 

26.07 

2S.96 

25.8* 

25. so la) 

2S.79 h> 
25,47 



Sanders and Dobbins, 

Massink, 
figures in 



are 



SOUIBILXTT OF !.irii' 



1 -^.0 

"3|8*O 

ij, |,7 

; i ^ 

r ,J,4 

6 S 7 

77 

0*1 - 9 
loo. i 
1 H . 

104.11 



100 t. vol. 

34$ ,76 t'-j) 1 

J5.3B 



Solid 



Li. 



.OS 



-H.il I l. iBjHu) 

j i.^ t i. 179) m 

,H . 7 J 

Ji.sst 1.176114) 



OF SPi.fi'tlc: Arm Af 



^rockfurci wti Wrb:,i*r, 
f OrAwford Ami rt>r<tn, 



IK Agt not'.s Stu.tTioH.s 



a. of 

ol. 

1.2UOI 



OBII, ptr tOO 

p. :U>!. Mi. 



0.0 



1.2712 1932 1^.74 

1.2992 15.82 21*73 

13.3^ aS*iCi 

10.42 38.12 

SOLUBILITY 01- 

Gms. per 100 Cm. Sat 



d.of 



H 8 S() 4 . 

5,05 22.74 

12,23 20.45 

16.60 19,10 

32.70 13.37 

42.98 10,57 

52,72 11,44 



i.,i. i J -r. 'M.-M I-iv* 4 MaJJCKILp 
.;iH ^.u sii.in "'* riH^L.B^O 

* t4ni. **,," * 



i .' . i * 

i i, if 



IiHJil 

itit;i 



Sri t \si IN AM. 



? i j 

^ AT 



II. H, 
fil 4(1 

C| 40 

vH n 



ij in) 
17 10 
tS Hi| 

. 75 
1 1 64 



^l?I I hf*. 

LiS() 4 



fy.4.1 *S r ^5 

SOLOEILITY OF LlTlltrM Sn,l-\tl'. IN AHHtrt I'tl Sn 1 1 ttr \t ID. 

ilirf^tw !u#* i 

10 ce. sat, solution in ilm, HS()| ftmtain J 71*1 HIH^. I ti^^* an* I thi* i isstalline 

solid phase has the coni|itisiiiit IJi^^.ylliHC^ tml iiirlf** at alxjtii u*' 

Kendall md lmdtm $ 



933 LITHIUH LI 

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 50. 

Gms. per zoo Gms. Sat. Gms. ir ipo Gnw. Sat. 

Solution. Solid Phase. Solution. Solid Phase, 

"TSSoI- (NH 4 ) s so 4 . 



M.T.1/2UW4. jw. a w v .- -.r. - ,..-. v i>r\ 

44 .! O (NHJjSOi 45-7 O (NH 4 ) a S04 

40*8 3 *3-S S-86 """""~ '""" 

an c 66 (NH<)2S0 4 "fNH4LiS04 10. 6^ l6.^ 

Oy J vr v ^ ^ V/*/ 

20 10 NH 4 LiS0 4 I3-90 21.20 

21.6 15 " 13-97 21.23 
15 20 " 11.45 21.75 

12.5 2T.9 NH4LiS0 4 -HLiiS0 4 .HaO () . 63 22 . 79 " 

8*9 23 Li 2 SO<.H 2 8.58 23. GQ 

o 25.1 " 7 S^ 22,86 

o 24.3 

Additional data for the triple points of the above system at 20, 57"* amf<)7* 
are given by Spielrein (1913), but the terms in which the results are prenenttul 
are not clearly shown. t 

Data for the quaternary system, ammonium sulfate, lithium miuatts alrohul 

and water at 6.5, 30 and 50 are given by SehreinemukerB and van l)orp (i<)<>7). 

A mixture of an excess of ammonium and of potassium sulfaton in water at 

19 was found by Riidorff (1873) to contain 37.97 gmn. (NlWaSOi -f 39,3 gsn**. 

K2S04 per 100 gms. sat. solution. 

SOLUBILITY OF LITHIUM SULFATE IN AQUEOUS ALCOHOL AT 30* 

(h'chrcinenmkrrs and van Dorp, Jr., 1906.) 

"* " ' ~~ ~ " "" " ~ " ~" Suit ,, ., t ril 

I Fhiwr, 



Gms. per ioojj 


;ms.Sat.Sol. 


Solid Phase. 


tims. per i<x 


:HttW, NU Nui, 


' QH 8 OH. 


Li 2 S0 4 . 




C 3 H()H. 


LigSC^ 


O 


25.1 


Li a S0 4 .HaO 


47.2E 


3,04 


II.7S 


16.16 


** 


5-50 


I .22 


21.19 


11.52 


u 


(KJ.3C) 


o . 3t|6 


29.40 


8.17 


a 


80/74 


o 


33-31 


6.66 


ti 


<)4 . 1 1 






Fusion-point data are given for". 

Li pSO^ * AgpSO^ (Nacken, 190710 

4- K^S0 4 (Nacken, 1907. ) 

" * Mn99* (Calcagni uad HAn>ttA 

" * NaS0 4 (Nacken, 1907,* 

11 + Sr) 4 (Calcagni and MArotiii, 191 j, I 

LITHIUM Ammonium SULFATE LiNH 4 80 4 - 

SOLUBILITY IN WATER. 

(SchreinemaJkerft, C'ochcr<?t, Fili^H) utt<l drWiul, iyoj, *1T) 

G 
t. 

O 

~ 5 

~io 2^..J " m -ic.K? ** 

it 

~2o.6Eutec. si.ts Ice+NHLLiSOi 70 16.18 " 



Gms. NH.LiSO 




l 


IJmi. NH 4 !*iS 


per 100 Gms. 


Solid Phase. 


t 8 , 


jrr it (imi 


Sat. Sol. 






Sill. Scil 


O 


Ice 


10 


35-25 


14 


it 


+-IO 




23-5 





30 


V^k 7 


29-7 


a 


50 


36 


: - 3S-IS 


Ice+NH 4 LiS0 4 


70 


36,18 



Li LITHIUM 934 

SOLUBILITY OF LITHIUM-POTASSIUM BULPATB IN WATER. 

(Spiel rein, 19*3.) 

Cms. per 100 cc Gmt, i^r ITO cc. 

t* Sat, Sol. Solid Phase. t*. ,_,i^iiM P ^ Solid Phase 

' 



tg ' 4 , 

20 t?6 3.6 LisSQi.KaSCX-J-LiiSOi 60 xo,6 16.3 

20 1^3 13.1 " +KtS(>4 QS 30.2 0.3 

60 32.5 6 " +iAsa 98 9 23 



SOLUBILITY OF LITHIUM-SODIUM SULFATBS IN WATER, 

(Sptelrtin, ipj.) 

Gms. per 100 ce. Cmt. p oo cc. 

t*. Sat. Sol Sdid Phase. 4*. ^^J^L^l^ Solid Pha. 

XisSOi. N%S0 4 . LitSO,, NrfM> 4 . 

o 31.4 5-9 US04,NatS04.slKiO+L^O 33-5 *$ x 
o 18.5 xi. 4 " "-HNWOi 33-5 3.Q 21,8 

7.5 20.4 a. 17 " (trfpbpt.) S3 2S x6 6 
16 32 9-3 " ** 53 16,7 27.3 

24 26 14.9 LWO|JNri|SO l .wW)-fltfO, 99 74 14-4 
24 16.5 21,4 " 4-NiiSCX 99 H-4 S.X 

32 20 x6.8 " (tripkpt.) 

There is some uncertainty a to whether til of the above results are in terms 
of grams per 100 cc. or per xoo gins, of wit. nolution. 
SeO LITHIUM SBLENITE ,J^^<>4-'HI,(, 

SoLUBXLXTY OF LlTIIIifM SF.I.KNITK IN WATI-H. ill*rnti-im and KCUUHO, 1921.) 



Gins. LijSeOj per ion gws. ui. *ol. ,,, H|.*i!t i !.;(> i.\.W 17.7*; 9,05 
LITHIUM SILICATE (ortlio) I.i 4 SiO 4 . 

Fusion-point data for mixture** of Li 4 Si t > 4 I Ca 8 Si < * 4 mid for Li 4 Si () 4 <f ZrSi() 4 
are given by Schwarzo ami Hmickt*, i*)i. 

LITHIUM ST ANN ATE Li,Sn(OH)r, 

SOLUBILITY OF LITHIUM STANNATK AND or IivfitiATKi> LITHIUM STANNATE 
IN WATKW, {XiH-hwr, fat,} 

SnO r , M |H ,,. 

43 'I.!* 

40 1,7" 

<)t ......... l.ftl* 

Ho....... 4. in 

LITHIUM VANABATB LiaVO^.iHjO 

SOLUBILITY OF LITHIUM VANABATK IM WATICK. i JUMwnhmm ml Hglin t i 




Urns. LiiVOj Ltirt. M*VO, 

pr lo (m. tUU4 tr ton m. Holltf 

t". l. not. t^tiMft. t" **i *| ibae, 

o.o a.4o Lt v V04.9lltO '18. j i.wj Li i |V0 4 .H 1 

20.8 4,60 * 4o.<> 4,w 

18.6 5,a > 4^.0 3,711 

3o.a 5.0r 5o,o v.8<> 

35.2 6,a5 w fio.o v.Tto > 

WQ LITHIUM TUNGSTATE Li t \\<) |4 

Fusion-point data for mixture* of lJjjWi) 4 J- K t WO 4 , Li a \VO 4 -f- Na, W0. v 

aad Li t W0 4 + W0 t are given by van Lkmpt, i<p r >, H0er*a 19^9* 

LUTETIUM see 



935 MAQHESIUH Mg 

MAGNESIUM Mg ' 

TH SOLUBILITY OP MAGNESIUM AND or MAGNESIUM ALLOYS 
IN AQUEOUS SALT SOLUTIONS AND SB A WATER. 

(Whltby, 19JH. 193K3.) 

A method based upon the oxygen absorbed and hydrogen evolution WAS 
developed. No absorption of oxygen could be detected but the evolution 
of hydrogen could be accurately measured in samples of gas periodically 
removed from above the corroding liquid. Large variations in rate of 
dissolution of different grades of Mg f containing varying traces of 
impurities in o.i n to 3.0 n NaCl and 0.05 n HCl,was encountered. The 
presence of 0.02 percent Mn causes an acceleration of attack with time, 
The rate of attack in sea water was lower, due to the presence of sul fates, 
Traces of saponin increase the rate of H evolution. Three magnesium- 
base alloys and one type of duraluminum gave substantially the same 
results as pure Mg. Non metallic impurities such as inclusions of 
nitride or oxide do not act either as cathodes or auclei far anodic 
attack in NaCl solutions. The initial rate of dissolution of Mg in 
H f O, cone, and dilute solutions of KC1, KBr, KI and K SO aad in *<ju*eoutt 
solutions of alkali is always practically the same. A theory of "primary 
preferential hydroxyl ion discharge" is proposed and supported by free 
energy calculations. 

100 gins. sat. solution of magnesium in mercury contain o.33 gin, Mg &t a 5. 

{ LoomK 1M1 i 

Data for the distribution of magnesium between aluminium and load and bKvwtt 
aluminium and bismuth arc given by Tammazm and Schuftmrnntcr, 



Fusion-points of mixtures of Mg * Hg are giveo by Ombi and Sperooi, 
1915. 

MAGNESIUM ARSENATE. 

Data for equilibrium in the system magnesium oxide, aroium* trioxido and wntir 
at 25 are given by Story and Anderson, 19^,4. 

MAGNESIUM BROMIDE MgBr f .6n f O. R 

SOLUBILITY OP NAGNBSXUN BROMIDI m 



MgBr, p.r 



100 






100 ^ 



- 3.92 i2.o8 Ice + 10,4 99.3 HgBr ,6H 
" 6*85 18.36 rt 19,9 will f " f 
-15-2 32.86 " 34,8 103*. 3 " 
"37.5 53.93 " 39.8 103.0 * 
-42.7 Rutec 58,20 " MgBr f .ioH,0 34.8 105.4 

-23.0 68.6 MgBr .loHJO 39.8 106. < 

" 15 - 7 3-<> " 60.1 na o 

" '' 78 ' 7 " 65.5 U4.$ 

7.0 79.7 * 100.0 U^.il *' 

- o. 83tr.pt. 97. 7 > MgBr^.61^0 172 ^ m * pt " t70 *' r 

d. of sat, sol. at 18 = 1.655 (Mylius & Punk, 1897,! 

The previous results of M/?nschutkia, ^06, are shown to ^ too low. 



MAGNESIUM ^3 6 

SOLUBILITY OF MAGNMIWM BXONIDI IN AQUXOUS SOLUTIONS 
or HYimoBROHic ACXB AT 25 . 

(Scott ma Durfc. wo.) 
w * 8olld 



o.o 49.93 MgBr, ; 6H,0 

4.70 4$40 ^ 

9.83 40.33 H 

14.79 3S*S5 

100 gms. sat. solution of Magnesium Bromide i li*ia Ammoaia contain 
0.004 MgBr, at o. iliniiard and Stephan, 1933, 1934.) 
100 cc. acetonitrile dissolve 13.35 gm*. Mg Br t at a5. iMultor, u., 1924.1 

100 cc. pyridine dissolve o49 gins. Mg Hr t at 18, o.5,{ gms. at a5<> and a.5 gms 

at 60. I MllUof R., J924 .] 

Fusion point data for mtxtur of Mg Br t {- K Hr wui Mg Br t -f NaBr'are 
given by Kellner, 1917. 

or HAjtsitjH BKONZOI IH ETMTL BTKIR. 



The author made a veqr careful tiudy of the factors influeRcing the 
accuracy of the results^ including the effect of moisture and of light. 
The very greatest care is required to obtain accurate results. The 
values are considerably lower thua those of Menachutkin. 
tot. gBr f ptr 8olU 

C 100 PW. <) Ph* l 100 



-20 0.32 MgBr f .s<C f H,) f O 30 3.50 %Br f 2(C ? H }0 

~io o,(o f< as 3.91 

o 0.70 ** w o a.o**1 

*-io 1.18 "* *io a^7i, Iwwlscible 

14 1.58 HiBr^atC^iyO 20 a-osf liquid Phase 

16 U g 4 ' 10 "i*9J 

18 a. n " 

MAGNESIUM BROMIDE ETHER ATES, ALCOHOLATES, ACIDATES, 
ETC. 

SOLUBILITIES RESPECTIVELY IN KTHKK, Au:oHot. f A<UDH, ETC, &T 

VAR>Ot7H TRMi*KltATtfitRH. 

(Boris N. Measchutkin. Mooocnpti In thf ttiwlitft rniiik*! *' On Kthntei ami Other Molec- 

ular Corobiwttofts of Mtgwerfum BntmUte nitt I*M|II|# " Si fVirnburit. *|o?, pp. fi? nd XLVHI. 
Abo pubiytidl In the Hewofat til tb"* Si.. Prirnrfturx t'ofvirclirtte ImtUutv. Vls. t -7, 1904"- 1907, and 
in cwidtittfid form in Vob. 49 4i of ite Ztit.. unarjc. <'h*m , t*w I 
Preparation of Material. Hit dif*ihtrnfe af magnesium bromide, 
MgBr 2 .2(CtHft)tO (Z.anorg. Chtm,, 49 ^i, *tx) w,w pr*(urcHt by the very gradual 
addition of bromine to a cole! mixture* of nuKtwHtum |xtwtlt*r and dry ether, 
It IB very hygroscopic and m stable only tincitr IIH nhrrral ttoltttion. It is decom- 
posed by water and react n with very niiny or^anu* cfmifMiundH an alcohols, 
acids, ketones, estera, aldehyde, etc. The* acirfttion product* thus formal con- 
stitute the material employed in the awbor'n <itirrriiiig f*fijlk % s, The mono- 
etherate of magnesium bromide, MRBr,K*iHM> wan prewired jut us the 
dietherate, but the temperature during cryHii!li**ttttm w,m k<*f>l alx>ve 30, at 
which point the dietherate ti con vert et I t> mom>etheriitr. It i** aluo precipitated 
by dry %r!!in, 

Method of Detemunation of SoteWlitj. Ai tcmp*raturi*H Ijelow 30 the 
determinations were made by agitating an of the* mill with the aolvent and 

analyzing the saturated notation. At the higher temperature* the synthetic 
(sealed tube) method of Alexejeff (Wied. Ann., 1885) was uiecl. 
See also Matftesiaw fodlde 



937 



MAGNESIUM 



MAGNESIUM BROMIDE 
ETHERATES 

SOLUBILITY OF MAGNESIUM BROMIDE DIETHEEATE, MgBr 2 . 2 (C 2 Hs),O AND OF 
MAGNEsmM BROMIDE ETHERATE, MgBr a (C 2 H 3 ) 2 0, IN ETHYL ETHER, (C JMA 
AT VARIOUS TEMPERATURES. 

(Menschutkin. Sec preceding page.) 



Solubility of the Dietherate 



Solubility of the Monoetherate 

in Ether. 



m btner. 
Gi-ns. per 100 Cms. Sat. Sol 


Mob. 
2(C 2 H 


MgBr a . 
)|Opcr 


r. 


.. , Mob.MBr,. 
GTTO. per loojGmt. Sat. Sol. (CHi)iJ) ) r 

i"*T"r ' ' //" "iJ \ 7\ " \Jt *H i_ IOO MOtt. 


t. -.T"^ it* u C \ MftUr "' 100 wois. MRJBrj.vv-aJfwav 
MgBrj.zCv-jnjjzU. ivigurj. g^ j.^ 


. ***n***a. ^^ ^^ 


8 


i. 08 


0.6 


0.24 


o 


68. 


8 


49- 


I 


28, 


I 


O 


i .44 


0.8 


O 


32 


20 


67. 


2 


47* 


9 


27, 


1 


+ 10 

14 

16 


2-3 

2.95 
3.48 


1.27 
i .64 
1-93 


O 
O 
O 


S 2 

.67 
.80 


3 
40 
60 


66. 

65- 
63- 


5 
5 
8 


47. 
46. 
45- 


3 

7 
5 


26. 
26. 

*5- 


6 

I 

I 


18 


\J 

4.14 


2-3 


O 


. 9 6 


80 


62.1 


44. 


3 


24. 


2 


20 


4.86 


2.7 


I 


.125 


100 


60.7 


43- 


3 


23, 


5 


22. 


8 6.3 


3-5 


I 


.6 


120 


59.6 


42. 


5 


22 , 


9 


Two liquid kyers separate between these con- 
centrations of MgBr 2 .2(QH&)3O. 


X4O 

158 


58, 

57 


S 

S 


41,7 
41 


22 , 
21 , 


3 

9 


23 
24 
26 

28. 


72-3 
75-3 
79-5 
5 84.2 


40.1 
41.8 
44.1 
46.7 


36 
40 
4 6 

54 


.8 
,6 

.2 


Two liquid layer! Migrate Itrtwccn ihcv! con- 
centration* uf MgBr s ,(C 8 iU s O. 

158 ;.8 4-15 1.6 
158 4-8 3-4 *-3 6 


3 


85.5 


47-4 


56 


.9 


159 

162 


i 




.90 

.38 


I 




.4 

.27 


O 



n 












170 


o 


.18 


o 


- X 3 


O 


,0$ 



At 22.8 and 158 the saturated solutions of the cliethcratc and monoethtjratc, 
respectively, separate into two liquid layers which have at the intervening tem- 
peratures the following composition. Determinations of the upcciftc gravity of 
the lower layer gave % 1.1628 and d^ * 



Grm. per 100 Gnu. Solution, 



t*. 


Lower Layer. 


Upper U 


yer 




MgBr 2 .2(C2Ha) a O 


. MgBrg. 


MgBiTaCCJHi)^). 


Mr,. 


10 


75-75 


42 


3-2 


i ,8 





73-9 


41 


4.1 


2,3 


+ 10 


72.2 


AO.I 


S 


2,8 


20 


70.8 


39-3 


5-0 


3-3 


3 


69.8 


38.7 


6.8 


3-8 


40 


68.8 


38.2 


7.7 


4 -3 




68 


37-3 


8-S 


4,7 


60 


67-7 


37-6 


9.2 


S-* 


70 


67.7 


37-6 


9-7 


5-4 


80 


68 


37-8 


to 


5 -6 


90 


68.6 


38-1 


10.2 


5-7 


IOO 


69.4 


38.5 


1O4 


S-8 


120 


71 


39-3 


10. X 


5-6 


I4O 


72.4 


40.15 


C).2 


S- 1 


158 


74 


41 


7-8 


4-3 



unstable 



Htable 



Br 



938 



Mg MAGNESIUM 

MAGNESIUM BROMIDE 
ALCOHOLATES 

SOLUBILITY OF ETHYL, METHYL, PKOPVL, ETC., ALCOHOLATES OF MAG- 
NESIUM BROMIDE IN THE RESPECTIVE ALCOHOLS. (Mciuchutkin, 1907.) 

These compounds were all prepared by the action of magnesium bromide 
dietherate upon the several alcohols. The ether was expelled and the new A!CO- 
holate addition product recrystalHzed from the respective alcohol. The solubility 
determinations were made by the synthetic method. 



Solubility of Solubility of Solubility of Solubility of 


MgBr 2 .6CH 3 QH MgBr 8 .6C a H$OH MBr*6C. jHrOH MgBn.6 IsoC 4 HiOH 
in Methyl Alcohol. in Ethyl, Alcohol in Propyl Alcohol, m IsoButyl Alcohol, 


Cms. MgBr 2 , 
., eCHjOH i. 


Gms. MffBrf. Urns, Mir 


B/a Gmi. Me Dr. 
t .. 60 4 H,QH' 


* per ioo 

Gms. Sat. Sol. 


pur xoo * Pr xo< 

Gms. Sat. Sol. Gms. Sit. 


$>l- Cms. Sat. Sol. 


o 42.6 o 


17,2 o 77, 9 


SS-8 


20 44-^ * 


24.9 * **$ 


xo 60. s 


40 46-7 20 


32.7 20 85.1 


20 65.2 


60 48.9 3<> 


4 3 3 SS , $ 


30 69.8 


80 51.4 40 


47. & 40 9^ 


40 74-3 


ioo 55.5 60 


62,2 43 93 


SO 78.5 


120 60.7 SO 


73-8 46 94-3 


60 82.4 


140 66.8 oo 


78.7 48 95,8 


^5 84.2 


1 60 74 ioo 


86.7 $o 97,8 


7i 88 


180 84.5 103 


$o siro.pt, ioo 


75 92 


185 88 106 


94.4 


77 94-6 


I9ora.pt. 100 108, 


.5m.pt, ioo 


8om.pt. 100 


Solubility of 


Solubility of 


Solubility of 


MgBrj.6 Iso CsHuOH 
in IsoAmyl Alcohol. 


MgBrt4(CH.)tCHOH u I%Br. 4 (CHi) 3 COH 
in Dimethyl Carbtnol. in Trimethyl Carbinol. 


Gm. MgBrt. 
t . 6C|HnOH per 


Gms. M|Br^ 


Gms. Mf Bh. 
f 4(CHUiCOH 


* * IQQ Gms. 


per too Urns, 


per too Gms. 


Sat, Sol. 


Sac, Sol. 


Sat, Sol. 


o 70.2 


o 40 


24.7m, jt, of (CH,)|COH 


10 75.6 


ao 43,2 


24,4 Eutec. 0.06 


2O 8o.2 


40 4$ 


25 i 


3O 84.5 


60 4B-S 


35 9-5 


35 86.7 


^o 53.3 


4S 19- x 


38 S8. 7 


ioo 59 


55 32.2 


40 go 


120 67.3 


60 40,5 


42 92 


130 74 


70 6a.$ 


44 94-2 


136 83,6 


75 77 


46 m. pt. ioo 


138 90 






139 m* pt, ioo 


So m. pt, ioo 



MAGNESIUM BROMIDE ANILINATES. 

SOLUBILITY OF MAGNESIUM BEOMIDB AKILIHATES IN ANILINE AT 

DIFFERENT TEMFIEATUISS, (MraKktukia, 1907.) 

The compounds were formed by the action of aniline on magnesium bromide 
dietherate. The three compounds were: MgBrt.6OH*NHt, MgBri4CiHNH a 
and MgBr*2C.HiNHt. 



Gms. M|Br t . 



I . 


per ioo Gmi. 
Sit Sol. 


IO 


3.2 


So 


$* 


70 


7-5 


90 


12.8 


xoo 


18,5 


103.5 


27.5 


103 tr. pt, 


24 


X2O 


24,3 


140 


24.3 



SoiW Fhw, 



$$& 

pr ioo Om. 



160 


a6 


180 


28,3 


200 


33-5 


220 


4$ 


230' 


SS 


237 tr. pt. 


76.3 


2$o 


77*3 


160 


78.1 


270 


79 



939 
BROMIDE 

MAGNESIUM BROMIDE PHEITSXHYDRAZINATES. 

SOLUBILITY OF MAGNESIUM BROMIDE. PHENYLHYDRAZINATES IN PHBNYL- 

HYDRAZINE. 

(Menschutkin, 1907,) 
(Approximate determinations.) 

s. MirBr,. 

Solid Phase. 



MAGNESIUM Mg 





Gms. MgBr2. 




Gms, MfiBrj. 

Rf* W KTMMW 





6C,H 6 NHNH a sdfo phasc> 
per ioo Gms. 
Sat. Sol. 


t. 


OV#*lftiN JfliN rl 

per ioo Gms. 
Sat. Sol. 


2O 


3 MgBr s .6QH|NHNHt 


ioo tr. pt. 


54-8 


4 


7 


140 


60.8 


6o 


16.4 " 


180 


68.4 


80 


33 


200 


73-4 


99 


54-8 







MAGNESIUM BROMIDE COMPOUNDS with Ben/aldehyde and with Acetone* 
SOLUBILITY RESPECTIVELY IN BENZALDEHYDE &ND IN ACETONES. 

(Menschutkin. 1907.) 

The compounds were prepared by the action of benzaldehyde and of acetone on 
magnesium bromide dietherate. On account of the nature of the compounds the 
results are only approximately correct. 

Solubility of MgBr^GHaCOH 



ehyde. 



Solubility of M* Bri.3CHi.CQ.CHi. 

in Acetone* 



Gms. MBr s . Gms. MfrBr,. 
to 3C 8 HCOH t . jCcHftCOH t 

1 * per too Gms. per ioo Gms. 
Sat. Sol. Sat. Sol. 


Gnu. MgBi|. 
aCHs.CO.CH, 

per too Gmt. 
Sat. Sol. 


r. 


nr too < itm. 
Sat. Hoi, 





-7 


140 


17.8 


o 


O.2 


75 


5 


3 


1.3 


US 


37-S 


3 


0.8 


76 


71.6 


60 


1.9 


146 


65 


60 


1-45 


80 


83-3 


IOO 


3-4 


148 


84-5 


70 


2 


84 


89.8 


1 20 


6 


153 


93-2 


73 


5-5 


88 


9S- a 


130 


9-5 


I5Qm.pt. 


too 


74 


14 


92 m. pi 


u IOO 



MAGNESIUM BROMIDE COMPOUNDS with Methyki, Oitho Ethytf0rmat 
Formic Acid and Acetic Acid. 

(Menschutkin, tyo/a.) 

The compounds were prepared by the action of methylal, orthocthylformtte* 
and absolutely dry formic and acetic acids on magnesium dietherate. In the 
of .the latter compounds the results are only approximately correct, due to their 
extreme hygroscopicity. 

Solubility of Solubility of Solubility of Solubility of 

MgBr a .2CH,(OCH 8 ) s MirBr,.2CH(OC.Hi)i MgBr,.6HCCX)H MfcBr.6C.HiCOOH 



in Methylal. 



Cms. MgBr 



per zoo Gms. 
Sat. Sol. 



0.3 
0.45 

0.6 

0.75 

0.9 



20 
40 

60 

80 

ioo 

106 

2 liquid layers here 

106 86.2 

108 90.8 

no 95.4 

112 m, pt. ioo 



t*. 

o 
20 
40 
60 
80 
90 

95 
xoo 

no 

1x4 m. pt. ioo 



:hylformate 

Gms. Ad[ERr4. 


. in Formic Acid. 

C*m> MK*rt 


m Acetic Acid. 

C(f\"i, MtjH: 


aCM(OC|Hj)j( 


to 


6HCOOH 


t' * 


0CII|CC501 


per ioo Gnu. 
Stt. Sol, 





per ioo Om*. 
Sat. Sol, 


. 


iwr ioo On 
Hal, So). 


II. I 


O 


49 8 


17 


0,3 


12.5 


ao 


57-S 


30 


i ,5 


14. S 


40 






4-S 


18.6 


60 


73 -s 


60 


7.Q 


25.7 


70 


70. 1 


70 


id, a 


35 


80 


86 


Bo 


3^*S 


41 


80 


95 


90 


57-7 


50 


88 m. 


pt. ioo 


xoo 


71.8 


66 






10$ 


Ho 


88.5 






HO 


%*S 



Br 



t m, pt. ioo 



Br 



940 

MAGNESIUM 

MAGNESIUM BBOMIDI COMPOUNDS with Acetamide, Acetaniiide and 
Acetic Anhydride. (Mewchutkiii, 1909.) 

The compounds were prepared by reaction with magnesium bromide dietherate. 

Solubility of Solubility of 

MgBr.6CHCONHCfHi MgBr a .6(CH 8 CO),0 
in Acetaniiide. in Acetic Anhydride. 

Cms. 



Solubility of 
MgBr 2 .6CHiCONH 2 
in Acetamide. 
Cms. 

4- M M 8 Hr Solid Ph^e. 

' TOS* 

8am.pt. of CHiCONHs CHjCONHs 
80 3-1 " 



MKBr t .6CHr 
CONHCHt 
per loo Cms. 

Sat, Sot. 



J - -*> \ >>* "AN^W/IVS 

in Acetic Anhydride. 
Cms. 



Solid Phase. 



XI 2 m, pt. of CH 8 CONHQHs 



70 
60 

50.5* 

TO 
oo 

110 

130 
150 

160 
165 



21.7 
40 

56 

57-8 

60.5 

65 

7I-S 

80 

85 
oo 

IOO 



no 
108 



X2O 
140 
XOO 
180 

200 
20$ 
207 
2O9 



3-7 
7-7 



*3-* 
*9-3 
25-5 
35-3 
S9-S 



CKiCONHCiHi 



o 
20 
40 
60 

CONHQH* 80 



1 20 
130 
*33 

136. St 



per ioo Cms. 
Sat. Sol. 
26.4 
28.7 
31.6 
35-7 
41.1 
48.4 
57-8 
69,8 
77 
85 

IOO 



loot 



Eutec. 



t m. pt. 



MAGNESIUM BROMIDE COMPOUNDS with Urethan and with Urea. 

(Menichutkin, 1909.) 

Solubility of Magnesium Bromide Solubility of Magnesium Bromide 

Urethan Compounds In Urethan. Urem Compounds in Urea. 

Cms. ., Jf m *v./% 



per loo GmH. 

Sat. Sol, 

49 rn.pt. of urethan 
45 *8.$ 



Solid Pha*. 



* 
35* 

SO 
70 
So 
90 
91-5 
Qit 
100 

no 
US 

120 
123 



43-3 
4S.6 
51.3 
56.2 
66.5 

6^4 

73-8 

80 

84.1 

oo 

IOO 



t". 

132 
126 

IK) 
114 



Solid Phase. 



MfBr,.6CtHCONHi 



' Eutee. 



1 20 
127 



160 

170 

171 



jr * 

SM. ^o 

m. i>t. oC mm, 

o, 5 

17.2 

at 8 

5* 24 ^ CO-CNH.J^MgBrt.eCOCNH,), 

35 

4S-S 

60 

58 
60,7 

71,4 
83.7 
06 
f tr.pt. 



" 4-MfBr,.4CO(NH J ), 



MAGNESIUM BROMATE Mg(Br6 y ) t .6H/). 

zoo cc. sat. solution contain 42 grams Mg(BrO a ),, or 0.15 grammols. 
at 1 8. 

(Kc>hlruch Siub. K. Akud Wi*t,. f Berlin), i, oo* f w4 



941 MAGNESIUM Mg 

MAGNESIUM FORMATE Mg(HOOO) p .alI 8 0. 

SOLUBILITY OP MAGNESIUM FORMATE IN WATER. 

(Ash ton, Houston, and Say lor, 1933.) 
QBS. Mu(HCOO) pr Solid 0*s. Mg(HCOO) ? per Solid 



100 



Phase 100 



Qkns. per 100 i 


ygns. sat. sol 


Solid 
* Ph&s* 


' HCOOH 


Mg(HCOO) ? 


0*00 
1$73 
31.28 
46.7 


12.23 
10.10 
8.01 
6.22 


MgiHCOOl^y) 



-<.<xEutec 14.0 Ice+Mg(HCOO) p .2H p O so 16.8 Mg(HCOO), .a!1 f O 

o 14.0 Mg(HCOO) 2 .2H 2 60 18.0 

10 14.1 " 70 19.2 ;; 

20 14-4 " 8 20 ' 6 

3 15.0 " 90 22.2 

40 15-9 " 10 2( *' 

SOLUBILITY OF MAGNESIUM FORMATE IN AQUIOUS SOLUTIONS 
op FORMIC ACID AT 25. 

(Dunn and Philip* 19M.) 

QMS. per 100 *o. sa&, sol. Solid 

r HCOOH ^MifH^T"^ rhlMlf p|| 

60.9 4*68 

76.2 3*19 

90.8 a. is 



MAGNESIUM METHANOLATE MgiCH^O)^. 2CH^OH, 

SOLUBILITY op MAGNESIUM MBTHANOLATB IN METHYL ALCOHOL. 

(QMinoc, 1935.) 

Q On. Hols. Mg(CH 3 0) p 

1 per loo HAS. sat. soluaon 

-20 0.07*1 

-20 0.118 

66 0.079 "* (decomposition begin) 

MAGNESIUM ACETATE Mg (CH,COO) a .4H,O. 

SOLUBILITY OF MAGNESIUM ACETATE IN WATIE, f Kivu f *l 

Cms, (ims. 

Mg(CH 8 COO) a ^ 

perlOOgrai. Solid 

t". sal. sol. Phase. t". 

~o.364.. 1.068 Ice 4,0.1,., ':K>. MgfGU 9 < 

~ o.53r.. 1.804 14.9... 17.97 

- i.o83.. 3,o8 7,4.9... ^9.6 1 
-2.179.. 5.92 35.0,.. 41,78 
-4-687.. ri.4') 45.0... 44-7<> 

- 9-99- * ^9-Bi 55.0... 49.46 

-i5 . a8 . . . '2,5 . oo -c(>8 . o . . . 6(1 . \ npiirox. m, pi. r 

-29.0.... - 34.5 



Mg MAGNESIUM 

MAGNESIUM ACETATE Mg(CH 8 COO) t .4HsO. 

EQUILIBRIUM IN THE SYSTEM MAGNESIUM OXIDE-ACETIC ACID-WATER AT 



Gms. per 100 Gms. 


Gms. per 100 Gms. 


Sat. Sol 


Solid Phase. 


Sat. Sol. 


Solid Phase. 


' CHaCOOH. 


MgO. 


CH,CX)OH. 


MgO, 




3-36 


I. 73 MgO 


3^-37 


7-99 


(CHaCOO^Mg^HtO 




2.93 ' 


3^.23 


8.18 


+s 


8.06 


4.21 " 


35-77 


8.17 


3.3.3 


12.46 


6-54 " 


40.87 


7.42 


44 


IS-46 


8 . 24 " -KCBkCOO^Mg.^ 


1,0 47-86 


6.74 


4* 


IS-38 


8.31 (CHgCOO^Mg^HaO 


56.16 


5.81 


M 


14.25 


7.24 


61.59 


4.68 





20.19 


7 -47 


69.13 


3-75 





22.93 


7.60 


75-93 


-8S 


M 


26.6l 


7-74 


82.90 


2.23 






2.3.3 - 2(CHiCCX)) 8 Mg.3CH8CCX)H.3HtO. More careful work in the w*ion 
of the double salt showed that a second double salt of the composition 5(CHgCOO)i 
Mg.ioCHjCOOH./HaO was obtained. This compound usually separated from 
the more concentrated acetk acid solutions. 

100 gws. Methyl Alcohol sat. with anhydrous magnesium acetate dissolve 
5.25 gw- Mg(CH 3 000) f at 13 and 7,50 gw. at 68.ao d <b.pt. ). (Henstock, 1934.) 

MAGNESIUM TABTRATK Mg(C4HiO).aVi H X O. 

100 cc. of sat. solution of Mg (C 4 HO c ).iV H t m water contain 0.76 gm, 

Mg (C 4 H 4 8 ) at 3o and 1.44 gnu. at 90. ( Ch*urj td Dhur, \m.\ 

SOLUBILITY OF ACTIVE MAGNESIUM TARTRATB AND OF RACEMIC 

MAGNESIUM TAKTWATE IN WATER AT SEVERAL TEMPERATURES. 

( Du)n)ux uml CuttAl, im, } 

Results for the Active Solt. Results for the Bacemic Salt. 



pe'rlOOfnw. ' Solid 
t*. sal. sol, Phaif, 

o o.54o MgC^H>0$*<|H|0 


r 


^Bri|m. " Solid 
Ml. iwt. Phase. 

. A.Xn) Mtr.n.H.n,. iAf 


12.5... 0.848 
25 i . 174 


ia.5... o,58a 
a5.o. .. 0.826 

o 37.5... 1.095 

in 24.35 K m3 - succinate at 15 and 66.36 

(Tarugi ftjod Chccchi, 1901.) 

CiHtOtMg.31!fO; rtcemie, CsHiOni 

EACH FOEM IN WATKE, 
md Cut tut, urn.) 
Bicemic Salt. 

Cm-, <;,,<>,<, Ms a Solid 
f, |nr l^ f nu f. MM. Pfef. 
Q o /\ A^ r^lf.O^Mr. ^ 


26 . 2 ... 1 . 220 -t-Xf C t ll 4 0.tM t 

37.5... i.oSo MgCiHiOf.aHtO 
MAGNESIUM SUCCINATE CJW 

100 gms. sat. solution in water conta 
gms, at 100. 

MAGNESIUM MALATK active, 
SOLUBILITY OP 

( Duboux 

Active Salt. 

(Jms. C 4 If t O^.Mf SoUij 
t*. p@r 100 gms. sat. ml I'hasr, 


12 5 a a8 *'*** o* * 




t 08 


a5 . o 2 . 54 


- 




87.5 a. 80 


37.5... 


...t.38 



Saturation was obtained by oonttnuous rotation lor 7 to 10 hours. 



943 MAGNESIUM Mg 

GNESIUM LACTATE Mg (CgHgO^ ) ^ 3^0. 

ioo gms. Methyl Alcohol sat. with anhydrous magnesium lactate dliroU 
(C H ) at 15 and 1.14 gms. at 66. i(b.pt. ) . (Henstock 1934.) 

3522 



AGNESIUM DiLACTATK Mg(C 8 H,A).6H,0 racemic, Mg(C.H 4 O 6 ).3^A 

inactive. 

ILUBILITY OF RACEMIC AND OF INACTIVE MAGNESIUM DlLACTATE IN WATER. 

(Jungllmchj 1912.) 
ioo gms. HsO dissolve 7 to 8 gms. racemic and 2,28 gms. inactive lactate at 15. 



GLUCONATE 



ioo gms. sat. solution of MglC H ll 7 ) p .3H R iu Water contain 7.8 gin.*. 
(C 9 H 11 ? ) 2 at 25. (May, Weisberg and Herrick, 1929. > 



kGNESIUM BENZOATE Mg (C fl H4COO) 2 ,4H 2 0, 

oo gms. H 2 O dissolve 6.16 gms. Mg(CH 6 COO) a at 15 and 19.6 gnw. at joo , 

(Tarugi und t*hro:hi, 1901.) 
oo gms. H 2 O dissolve 3.33 gms. Mg(C HaCOO)2 at 15-20. (Squire and cine t KJO.V) 



ioo gms. Acetone sat. with anhydrous Mg betuoate dissolve 3.^8 gm 
;C fl H 5 COO) g at 15. (Henstock, 



^GNESIUM BENZOATE Mg(C 11,000),. ,fH a O. 
IGNESIUM .f-lNitro BENZOATE Mg(G a H 4 .N0 2 .COO ), JilUO. 
cc. sat. solution of Magnesium benzoaie in water j 

ontainC.364gms. Mg(C s U 8 COO), at . v,o. ( , ffl , , till t , 

cc. sat. solution of Magnesium 4-Nilro henzoate in ( *** limlm mtl wutw tfl|& 
'ater contain i.8/[o gms. i\!g(G fl n^NO a COOh at v.o e * \ 



3NESIUM BENZOATE Tri Methyl Alcoholate Mg ( C 6 

LOO gms. Methyl Alcohol sat. with the tri alcohoUtt* dissolve* uai 

5. M glC e H 5 COO) p at 15 and 70.98 gms. at 71.9" <b.pt.). (Hensiock, u>- 



iGNESIUM SALICYLATE MK(C 7 HiO,)j.4HsO. 

oo gms. sat. solution in water contain 20.4 gms. salicylate at !< (14, 

ure and Games, 1905), and 79 7 gms. at ioo* (Tarui ^ cbtcrW. ,> 

oo gms. 90% alcohol dissolve 0.6 gm. sahcyiate at is^so . (Squire *ad Cabei, 1905^ 



Mg MAGNESIUM 

MAGNESIUM PHTHALATE jMg C fl H 4 ilTOi ? , uH ? 0. 

S0LHBIUTT OF HAGNBSSMN PTMALATg in AqtflAflft SOLUTIONS 

OF PHTHALU* ACID. 

(awjttt ana Kly, i:)'%ij 

Ctea. per 100 jpt. *(. wl. 

w ____,.,,.,,., 



0.0 


30*6.3 


0.39 


30*78 


0.47 


26*58 


0.76 


16.20 


i.o6 


7.69 


1.58 


1.95 


1.00 


0.99 


0.29 


0,0 


0,0 


1*1 . 1! 


0.47 


3*1. t f 


1.03 


VI . 36 


1.16 


Vl0 


1.21 


33*36 


1.30 


40,98 


1.36 


27,119 


1.54 
1 .60 


2^.49 


1.72 


30.46 


1*79 


1*1*17 


2-33 


8,93 


3*23 


4.7! 


3.61 


4* 16 


2.70 


2.66 


1.69 


1.37 


0.69 


0.0 


0.0 


,.* 


3*53 


43.HO 


3*^7 


4 1 1 1 9 


3.88 


tf..VS 


$."$2 


JtJ.30 


6.56 


18,73 


7*95 


1 F l . 6H 


10.21 


U t> 


9.47 


9-95 


7*43 


6.9^ 


6.15 


5.36 


4.13 


j.% 


1.72 


0,0 



dll 



uH 



C HXX)HJ 

4 



A I n w 

3 M U*' <| H 4 ait) J .i ill /I 

" * MIHI'I 4 .8H,0 
MljlHPl,.KH f O * *' 



Mg(HP) f .BH,0 = 



GNESTUM HANDELATE 



945 

(r), (1), Mg(C fl H 5 CH<OH)COO), 



MAGNESIUM Mg 



SOLUBILITY OF MAGNESIUM MANDBLATBS IN WATER. 

(Flndlay and Campbell, 1930.) 



cms. Mg ( c 6 H 5 CH(OH)Coo )? 
per 100 gp.8. H g O 

'Besuits for Results for 1 
r-Salt 1-Salt 



,..m 
Solid R.M. 

iu solution* 



.52 
.36 
.15 
.06 
.04 



1.60 MgCMan) ? Jl g O 
1.68 " 

Q'72 
.77 



1. 
1.83 



Mg(Man) ? .4H f O 



0.95(2.61) 1.97(6.08) " 
0.88 2.11 Mg(Man) g 

1.16 2.72 " 



1.33 



5-07 



Results (i) for Solutions 
u ilibrium with solid 
p^^ composed of both 

active and racemic Salt. 
^ &m ptr loo ^t. HO 



o 

5 
10 

15 
20 

25 
30 
35 
40 



1.94 


0,24 


2. 12 


0.55 


1.59 


0.32 


2.66 


0.60 


2.23 


0.39 


1.96 


0*41 


2.16 


. 49 


2*40 


0,49 


2.SO 


O.$0 



an = C H CH(OH)COO 

i) Determined polarimetrically 

ther values for the solubility of the (r) and (1) salts in water are 
follows. 



16 
18 
25 
25 



CH 



1.8 
2.61 



4.5 



6.08 



McKenzie, 1899. 

Ross and Morrison, 1936. 

" " " and John stone, 



oss and Morriso.n, 1936 also give results for the system Mafnesiww Ir) 
delate t (r) Mandelic Acid HO at 25 in which lh acid salt, 
(C-H-O.I^C.H-O-.aH.O is formed. 

o7*5o7<3 r 

loss, Morrison and Johnston, 1937, give results for the system Magnesium 
Mandelate + (1) Mandelic Acid + l! a O at 25 in which the acid salt 
ch is formed probably has the same composition as that of the (rJ com 
nd but, due to analytical difficulties, metjuuabiiiiy *d slowness with 
ch equilibrium is attained^ conclusive results were not obtained, 

}NESIUM CINNAMATE Mg(C e l! B CII.CHCOO) t . i or * 11,0(7). 

SOLUBILITY op MAGHESIOM CINHAMATI in WATI. 



15 
18 
20 
oo 



Ott*. Mg(C H-CH.CHC00)., 
par 100 cc *2u aoluubo 



Authority 



0.85* (Tarugi and Checchi, 

1.114 (Fredhoim, 19344) 

1*225 (Ephraim and Pfister. ) 

1.94* (Tarugi and Checchi 



: per 100 gms. sat. solution. 



Mg MAGNESIUM 



SOLUBILITY or HAGMMXWH CIHHAMATS IN AQUEOUS SOLUTIONS 

OF AMMONIUM CHLOIOS AHD AMMONIA AT 18. 

{fffdftol. t*)34.1 

Coap. of Aq. aolvtnt 0*. EqMlv. Hg pr Coup, or AJ. olvmi On. Equlv. Mg per 

in Om. Equlv. ptr littr Uutf MI. ol. in <* Kqulv. pr lUtr Uur u. sol, 



Water alone o*07 o.aow* 4 ^* l o,s9S8wn 3 0.0957 

0,2994 NH Cl 0.08^7 o.94 " * 0.798 " v 0.0981 

0.2994 * * 0,1996 NH 5 O.OSS^ 0.299* " * 1.000 " 0.1004 

0.299q. fl *" 0.3992 H 0*0928 



MAaNBSIUM CAMPHOEAT1 (\!l t AMg.i4HiO, 

SOLUBILITY OF MAGNESIUM CAMPHORATK IN d C'AMPHORIC ACID AT 15 
AND Vu'K VKRSA. 

* h ami L^ftii r ie u , i y 1 4 , ) 



Cms, per IPO Cms. Stt Sol SolW ?to*. SKit Phast. 



0.622(13.5) o CwHiiOi 3.16 1030 

1,20 1.29 " 3-S *> 5 

I.9B 3 -S3 J< 3 ( ' * Ci 7 

2.36 5.66 " I *)t 5 * 

ails S.X9 M o 14-35 

CH 



MAONESIUII CAHPH0R CARBONATR 

SOLUBILITY op MACSHISI^H CAHIOR i*Aii>HAT IK ALCOHOLS, 
(Picon, 19*1.1 



, pr Llitr MI., sol, 



Methyl Alcohol CH Off io.s u>.^ 

Bihyl Alcohol C R OH > o. 16 



MAONKSTUM Alky] 



or EACH HXPARATILY IH VATIR. 

|R*fti wa TAfwr* if an,. | 



Magnesium n Decyi Sullonaie HgfCH ICH 

MgCCHl(CH* 



Myristyl w 

Cetyl w MgtCH,(CH 

OctAdecyi w * 



gtr tOO i 



o . 368 

gO.0,13 48.0 

0*001l5 0*0 16 

0.006 
JlgO.ocna 0.003 



94? MAGNESIUM Mg 

1ONBSIUM Anthracene, Benzene and Naphthalene SULFONATES. 

,-, iri . "\Ttf . _~-^ 

M 

Crw. nhydro<ii cmpd. 

per HK cc. ifll, * 





( Ephraim and Pftstor, 1925, 192 


5 <z ; Ephraim and ."agw, 19*5 




Compound. 


Formula. t"> 


gnesium 


Anthracene~i~sulfonate.. . i 


Jgic'nfot'vno w"." 









)> 




20 .... 




>) 


n 36,... 





)> W ....*. 




)^ 




n 65 ] ... 


>} 





8o.5.. 


J> 




8*1,0. , 


> 


Naphihalene-i -sulfonate. . 




> 


-2- ft 


UiCjo'^sOj^.-vt^o 16 . 5 . . 


> 


-y- " . . ft 


ImiWtSO,,.nH t <) 'K).(>. . 


> 


)> > 


3 '2 


> 





45 








5 9 








74 








i> 87. 



0.0799 

o . 0077 



7.639 
n.i53 



26 . Bt>4 
6.978 
<> . v, 

o.*H73 
0.490 
0,790 
i . 3,16 

,> 8* 

-6 oxy-'2-sulfonate . . 

Results for the solubility of Magaesium Bazen ._ 

aqueous solutions of Benzene Sulfonic Acid at 2S, are CH 

ven by Dunn and Philip, 1984. 

SOLUBILITY OP MAGNISIITM NAPHTMALIMK -3- SULFONATE IH AQWIOHS 
SOLUTIONS OF AMMONIUM CHLORIDE AMD AMMONIA AT i8 



apoaitlon of AQ. Solvent On. Kquiv. Mg per rouipooiaon of A.I. 

ft 0m. Cqulv. per liter liter aac,. sol. Jin On. Cquiv. per lUcr 



uer alone o.oio 0.1984HH 4 C1 * 0*784 PiMf 0oi?o 

NH 4 C1 o.om " " -* uooo 0.017$ 

11 * o.)96NH n 0.0151 0.2976 M O.OlS^ 

11 f 0.392 "' 0.01S5 H 4- 0.393 " 0.0166 

" t 0.588 " 0.0l6l " " + l.OOO * Ot 019 * 



AGrNESIUM Naphtliylamine Di SULFONATES Mg(.: lfl H|(NiIs)(HOa i 
a. 6. 8 and 2.6.7. 

o gms. sat. sol. of the 2.6.8 cmpd. in water contain 8.7 gms, ) 
MgC 10 H B (NH t )(S0 8 \at i5\ ' flimmnrhw^, 

o gms. sat. sol. of the '2.5.7 cmpd, in water contain 11,09 gm<t, [ i**** iw*i 

MgC JO H 5 (NH 2 )(SO a ) 2 at i5>. ' ) 

One liter water sat. with Magnesium- i-Naphthalamine a-*r7 
ntains 193 gms. Mg C 10 H.NH,(SO,),H at 20 and 235 gm- *l 

iu ^ r a ? < 



Mg MAQNE3IUM 

KAQKESIUK Aathrwlao<' SULPOXATRS 



or 



C H 



u$ Di&itoAt* 
us 

1*6 



ft.* 

l5 



stro*rfs 



CH 



XAOMK8IDM . 



, 

18 

'3 



100 

iff 

tl 

18 



8 



40-0 



0.31 



** 100 



,,! l-l SELBMATKH 
SouiMtltr . !: , w 



' 






o. 85 



* 



Alcohol 



Illtr 



** J | l#fc 

W * Mb mlmim HT 



fluluuon 



30 

feu |l* 



ft* 
'pi* 



0*37 



0.034 

0*01 



o.o ( = H a u; 

i8.i3 0.969 

28.37 0.9535 

45.67 0.9194 



949 MAGNESIUM Mg 

MAGNESIUM ERUCATE G a II, 7 ClUCH(CII a )iiOOOMg. 

SOLUBILITY OF MAGNESIUM EKUCATE IN AQUEOUS ETHYL ALCOHOL 
AT 25. (Thomas and Mattikow, 1926.) 

</ of (JftW. (! H IIj;(;H : (ill iCHvjin.OOOMg pet 1 

7 iinillilliiM iiiiiilllllliliin - 

Wl. por coiUjyijOII. Sl. sol. too cc. (. nol. 100 gini. folvon' 

.(>()() O.OOf) 

. 007 o . 008 

, o 1 9 o . oy.o 

(>5 . 8'i o . 87^4 < . 1 4'>. 0.171 

76.40 o . 85c>4 o . 1 79 o . y4o 

88.38 0.8177 o.?,6'8 i). 349 

94.28 0.80 1 8 o.'lv.H <>.<v,<> 

MAGNESIUM HEL.IANTHATE Mg(G u H u N a SO 3 ),.4II,O. 
100 cc. H 2 dissolve o.o35 gm. magnesium helianthate at ao-a5. 

(Stark wnd Dohn, 1918.) 

MAGNESIUM LIGNOCEEATE. 

100 gms. H a dissolve 0.002 gm. magnesium lignocarato at v.5. 
100 gms. 44- ! 3 per cent aq. alcohol dissolve o.oc>3 gm., and 100 gin. <jf,53 pr 
cent alcohol dissolve 0.006 gm. (Thorna* und Yu. 1023.) 

MAGNESIUM OLEATE (CH 8 (CH2),iCH:CH.CHsCOO) a Mg. CH 

One liter HjO dissolves about 0.23 gm. olcatc (soap). (Pahrion, 19*6,} 

100 gms. glyccrol (d 1.114) dissolve 0.94 gm. oieatc. (Amelhi, 7,i) 



MAGNESIUM OL.EATE ( C nl ll n (}() 

Solutions prepared by rubbing magnosiunx olaato (prupannl From technical 
sodium oleate) with water or salt solution and allowing to utand at room tompcruturft 

for 36 hours, contained from 4.28 to 5.4* milligrams Mg per liter of water and 5.85 
to 5.77 milligrams Mg per liter of o.o5 or o.i per cent aquaous Na Cl solution. 

{ 'Mnk ftml Linn*, If , | 

Solutions prepared by heating a upeniion of nmgnesium oleate in water c*r 
aqueous salt solution to the bailing point and allowing to eool, contained 
5o.6 parts Mg per liter of waJLer, 99.89 parts Mg per liter of o.l per <*tnt iiff, Nn CJ 
and 90.26 parts Mg per liter of o.i per cent a<j. K CI solution, (ituupt, m\- 1 

too gms. 63.07 wt. 0/0 aq. alcohol dissolve 4%(iu gm. (On U^dOO ^Mg lit * * 

') 7^.17 ' . (j.fl/l 

86. 1 6 .. H.o 

(ThomM KD| Yu liaa. j 

MAGNESIUM PALMITATE (C 18 II 3 |<!OOj, ."Vl^. 

Solutions prepared by rubbing magnesium pahmtata (prepurrd from pure sodium 
palmitate) with water or aqueous unit solution and allowing to stand at room 
temperature for 36 hours contained from ?,.8v, to 3.'i milligramn Mg per litrr of 
water and S.io, to 3.o3 milligrams Mg per liter of 0.05 to o. to per eent aqurous Na (U 
solution. ' (2i|lk Wld I4w% lt|jV; 

Solutions prepared by heating a suspension of magnesium palmitmte in witter 
or aqueous salt solution to the boiling point and allowing to cool, contained 
55.68 parts Mg per liter of water, 92,21 parti Mg per liter of o'.i per cmtt aq. Na Cl 
and 72.89 parts Mg per liter of o.i per eent aq. K Cl. I umtpt , iH j 



Mg MAGNESIUM 950 

MAGNESIUM STEABATB (H n H^OOOfeMif. 

Solutions propami by rubbing magnesium stMtnttn (prwpnrMl from commercial 
sodium stearate) with water or salt solutionsami allowed to stand at room temporatuj 
for 36 hours contained from 3.17 to *LaS milligram* Mg pr liter of water and 3 -70 
to 3.84 milligrams Mg per liter of .o5 to 0,1 % aq, Na Cl. solution. 

(Zink and Liorc, 1915.) 

Solutions prepared by heating a HUttpwiftion of rnagnosium stearate in water 
or aqueous salt solution to the boiling point and allowing to cool, contained 
66.89 parts Mg per liter of H t 0, 95.79 parti Mg per liter of o.i % aq, Na Cl solution 
and 99.62 parts Mg per liter of <>. I % aq. K Cl notation, , Hjull>t 1{m 

SOLUBILITY OP MAGNESIUM STSARA.TI; IN AQXJKOUS SOLUTIONS OK KTHYL ALCOHOL 

AT . % J. fThtimiM unit V, 



Constant agitation was employed for obtaining saturation 

Wi, percent C,H,ON 

III NOlVMtt. i/|\ *rf ftftt. 0l. 

o.o (ss H t O) 0.99709 

19-9-"* 

<7^9 

44-i3 ,. 

63.07 (1.87783 

72.17.,,. . ., o.H5&n 

86.16. , o. 8*4356 

CU 91 , 53 o. 8093$ 

MAGN1SIUM UtfBATB, KYBISTATl, FALMITAT1 arid STMEATI. 

SOLUBILITY OF EACH IN SEVERAL SOLVENTS. cjctit ami iMmm, 1916,) 

Cms- Each Salt lleiwmiiwti Separately per 100 (inu. Solvent. 




Solvent. 


t*. 


M Iau.f4t<f 


MX Myr^tu 


M Pittmitate, 


MIC Stearate 






<Ctt iBV x>>r 


<c tt Hgax>) r 


(i a>t>Vifli!!" 




Water 


^5 


0,010 


O.OQ^ 


0.005 


0,003 


i < 


3 S 


0,007 


0,006 


0,008 


0,004 





35 


0,010 


0,007 


0,006 


0,007 


" 


50 


0.026 


0,014 


0.009 


0,008 


Abs. Ethvl Alcohol 


IS 


0.5x9 


0,158 


0.034 


O.OI7 




25 


0,591 


o, 236 


0.058 


0.023 


" 


35 


0,805 


0,373 


0,085 


0,031 


Methyl Alcohol 


50 
IS 


1,267 


^577 
0,571 


0,151 
0,227 


0,084 





25 


1,'ioS 


0,763 


0.36 


0.100 




$x.S 


* * 




0,50 


0,166 


Ether 
Ethyl Acetate 




0,015 
0.004 


o.oxo 

0,004 


0.004 
0.004 


0,003 
0,004 




35 


0,011 


0,010 


0,007 


0.008 




So 


0.024 


0,021 


0,013 




Amyl alcohol 
it 


*$ 


0.191 


0.086 


0,043 


0.014 




25 


0.236 


O.X45 


0.066 


o.oiE 




35 


1.481 


0,438 


0,104 


0.039 


Amyl Acetate 


5^ 


4.869 
0.119 


O^J 


0,263 
0.039 


0,105 
0,029 




25 


0*162 


0.073 


0,045 


0,030 


41 


34*6 


0.259 


0,105 


0.057 


0,046 




S 


1,939 


0,605 


0.216 


0.11x5 



951 



MAGNESIUM 



t. 

48.7 
ss 

S 8.i 

69-0 

77 -8 
87.4 
90.0 

93' 

96.4 

xoo. o 



BoUd PhftM. 



MAGNESIUM PLATINIO CYANIDE MgPt(CN)^ 
SOLUBILITY IN WATER. 

(Buxhocvden and Taraman Z. anorg. Ch. 15. 3* ? 9?0 

Gms. MgPt(CN>4 
per looGmi 
Solution. 

40.89 

4^-33 
42.15 

43-40 

44-9 
4S-S 2 

4S-6S 

45-04 

en) 96 . 4 

MAGNESIUM FerroCYANIDES. 

SOLUBILITY IN WATER AT 17, 

(Robinson, 1909.) 

One liter sat. sol. contains 1.95 gms. magnesium potassium fcrrocyankhr. 
MgKtFeCiNt. f 

One liter sat. sol. contains 248 gms. magnesium ammonium ferrocyaruut*, 
Mg(NH 4 )2FeCNe. 
MAGNESIUM CARBONATE 



Gms.MgPt(CN) 4 
t. per xoo Gms. Solid Phase. 
Solution. 


-4.12 


24.90 


MgPt(CN) 4 .6.fr-8aH20 


o-S 


26.9 


(Red) 


5-5 


28.65 


u 


18.0 


32.46 


l 


36.6 


39-53 





45 'O 


41-33 


** 


46.2 


42 .0 





42.2 


40.21 


MgPt(CN) 4 .4HaO 


46-3 


39-3$ 


" (Bright Green) 



44-33 
44 .o 



MgPt(CN) t .HjO 



SOLUBILITY OF MAGNESIUM CARBONATE IN WATER AT 25 
AND PRESSURES or CARBON DIOXIDB CJP TO ONB ATMOSPHERE. 

(KUn, W0J 

The saturated solutions were prepared by bubbling mixtures of carbon 
dioxide and air in constant proportions through conductivity water io 
contact with finely divided solid for periods of three to five daya. 



Partial 
Preaur 
or C0 ? in 
ACrtospharea 
0.000107 
0.000113 
0.000170 
0.000179 
0.0001Q7 
0.000210 
0.000233 
0.000251 
0.000310 
0.000376 
0,000380 



Ml 111*01 a par 1000 aM* H ? 

[Hg~J [HCO "J [flo""0 

w * ? * 

0.00^33 0.004880.00189 

0.00445 0.00501 0.00195 
0.00577 o. 00745 0.00205 

0.00593 0.00763 0,00212 

0.00658 0,00795 0,00361 
0.00708 0.00806 0.00305 
0,00780 0.00837 0.00361 
0,00807 0.00855 0.00380 

0.01013 0.01184 0.00421 
0.01296 0.01404 0.00594 
0.01355 0.01432 0.00639 



Partial 




0.000510 
0.000680 
0.000845 
0,000887 
0,000930 

0.00334 
0.00690 

0.04321 
0,lll6 



0,01437 0,01710 

0,01512 0*01873 0,00376 

0.01566 0.01990 0*00571 

0,01S93 0*02046 0,00570 

0. Ol6ai| 0,03119 O.OOS^S 

0,0l859 0.02698 0.0QtO 

0.02310 0.03548 0.00436 

0*03507 0.0446S 0.00371 

0.03127 0.06032 0*00116 

0.04601 0.0ft99B 0*00103 
0.06a66 0,1236 
0.2135 0,<|369 



. 968n 

The activity product constant of magnesium carbonate at as is token 
as i x io~ 5 and that of magnesium hydroxide similarly as 5 x 10" IJ> , 

The author also gives the following interpolated values of the nol*riiy 
of magnesium in a-jueous solutions saturated with HgCD s .3H f O &i as and 
at partial pressures of Carbon Dioxide up to 15 atmospheres, 

Partial Pressure Mllliaola (tf(O Partlti Praairi HUUnwJ,* (HJ 

of CO^ in A una. pr tOOO Una. *y> of CO^ In ACM. par 100Q $w W^9 

0.001 0.0178 0,7 O.lSl 



0.01 
0.05 
0.10 
0.3 



0.0270 
0,0489 

0.0660 

0. 117 



0,7 
1.0 

2.0 
5*0 



oai7 
0.387 
0*384 
fi . 11 * 



Mg MAGNESIUM 952 

MAGNESIUM CAKBONATE 



SOLUBILITY OF MAGNESIUM CARBONATE IN WATER CONTAINING INCREASING 

AMOUNTS OF CARBON DIOXIDB AT t5. f Mitchell, 1933. ) 

A silver lined steel bulb was usftd. The mixture was stirred by a current of CO 

Unfit. ir tiler of sat, sotation 

|J f^mam^m 

tula) i 



Atmosphere* prossun 
of (nrtan Dioxide. 



II. 

i3. 




.738 



RQUXlXBRXim IN 1MB SYSTEM MAGHESIUM 0*I0t. CAKBOJf DiOJUDE AWD 





(i*of 


Om* per tOO pa. Solid 




t 


a at. 


0ft U Ml* Pb*t 


i 


-1.80 


1.041 1 


3,410 1.536 MgOOg.sHjO 


30 





1.0407 


3.219 


.496 


as 


+5 


1 .0395 


3*942 


.433 W 


30 


10 


1*0383 


J.96a 


363 " 


15 


is 


1*0373 


2.744 


.^ 12 w 


40 


20 


1-0363 


2.606 


256 


41 


5 


1.0407 


3.&3a 


530 MgCO g .3ll 


50 


10 


1.0360 


3*736 


114 w 


55 


IS 


1.03^0 


2.270 


143 


60 




J.I 09 0.^856 MfQ0 8 ,3H 

0350 1.839 0.8654 w 

1.572 0.7634 " 

1.381 0,6780 " 

i*ao6 0.6017 " 

1.044 0.5333 w 

093a 047lfi " 

0*833 0*4083 w 

0*746 0*3648 M 



.0170 

*ons 

,0097 
0050 
*0008 



0.9080 

Results are also given for tht solubility of $MgQ.uOO t .7H f O In Water 
saturated with OP f at one Atmosphere pressure, 

Data for the syste HgO * MgCl^ * K^D at 25 and at 50 are given by 
Magda and Yawane, 193*8. 

Determinations of the eiuittbriw ia the systaw M|00 f t 00 f t HO wade 

by passing 00 at Atmospheric pressure through mixtures of H f O 4- %D 
and K a O * Mg s C0 3 at temperatures from o y to 40, Are given by Tereda, 
1928. There is 1 however,oe uncertainty in regard to the exact tenwa 
in vrhich the results are tip reused. 

SOLUBILITY or HAOMKSIUN CARKOHATI in OD f Pttt WATI* AT 100. 



The determiniiilons showed that o.ojo p. HgO = 0,063 l w * M0^* P er 
liter was dissolved at 100. It was found tbAi the solubility ts in- 
creased by KaCl ad Na^SO.. Na^l ud Na f Ct) n do not reduce the solubility 
of MgOO as much as they db that of tUOO .*' Results for the simultaneous 
solubility of MgOO^ and CaO^ la WAI^T a? 100* show that with increasing 
time of boiling, fron ik to 48 hour:*, the dissolved Ca0 increased about 
S times while the dissolved MgO decnsueft About i*** liw^s. The results 
are of interest in connection with ib* purificAiion of boiler waters. 



953 MAGNESIUM 

MAGNESIUM CAEBONATE MgCO,.3H a O. 

SOLUBILITY IN WATER IN PRESENCE OF CARBON DIOXIDE AT 15. 

(Treadwell and Reuter 2. anorg. Ch. 17. aoo, '98.) 



cc COzpertoocc. 
Gas Phase (at o 
and 760 mm.). 

18.86 

5-47 
4-47 

I . <A 


Partial 
Pressure of CO 2 
in mm. Hg. 

143-3 

41 .6 

33-8 
11.7 




Grams per 


TOO cc. Solution. 




r Free COa- 
O.IlpO 
0.0866 
0.0035 


MgCO 3 . 
0-0773 


MgCHCQft. 
I.2I05 
I.2I05 
I.2IOS 
I .0766 


Total Mg. 

0.20x6 
0.2016 
0.20x6 
0.2016 


A OT- 
I -H 


10.3 


. . 


0.0765 


0.7629 


0.1492 


OJ 

I .o7 


8.2 


. . . 


0-0807 


0-59S 2 


0.1224 


* ' w / 
o -62 


4.7 


* 


0.070! 


0.3663 


0.0865 


0-60 


4.6 


* * 


0.0758 


0.3417 


0.0788 


0.33 


2 -5 


. . . 


0.0748 


0.2632 


0-0655 


O-2I 


1.6 


. * 


0,0771 


0.2229 


0.0594 


O-I4. 


i.i 




0.0710 


0.2169 


0.0566 


\S * *f 

o.oi 


0-3 


* 


0.07H 


o . 2036 


0.0545 


V 'J 







0.0685 


o . 2033 


0.0536 







* 


0.0702 


0.196 


0.0529 




... 


* * 


0.0625 


o . 2036 


0.0520 








0.0616 


0.1954 


0.0511 


... 


* * * 




0.0641 


0.1954 


0,0518 



Therefore at o partial pressure of CQs and at, 15 and mean barometric pressure, 
one liter of saturated aqueous solution contains 0.641 gm. of MgCOt plus 1-054 

It is pointed 'out by Johnston (1915) that although Treadwell and Reuter made 
very painstaking analyses, their mode of working did not secure equilibrium con- 
ditions, a fact which is borne out by the lack of constancy of the calculated solu- 
bility-product constant, 

SOLUBILITY OF MAGNESIUM CARBONATE IN WATER CHARGED WITH CAR- 
BON DIOXIDE AT PRESSURES GREATER THAN ONE ATMOSPHERE. 

(Engcl and Vilk Corapt. rend. $3. 3o, '81; Engel Ana. chim. pkys. W *3t J4^ '.) 



Pressure of p. MgCPa* per Uyr. ^IxMtt^ ^^JllJlg^^I H^TI 

Atmospheres. At xa. At 19. ' Atmoiphem. Al '^ Al *^' 

0.5 20.5 ... 4-o 42.8 

i.o 26,5 25.8 4-7 43-5 

2.0 34-2 33. i (2. i At.) 6,0 50.6 48. 5 (6. a At) 

3.0 39.0 37. 2 (3. 2 At.) 9.0 ... 56,6 



SOLUBILITY IN WATER SATURATED WITH CO a AT ONE ATMOSPHERE. 

(Eagtl.) 






Gms. MgCOs* 


ty 


Gm. MgCO/ 1 




Cm Mt'C 





per Liter. 





per Litfi. 


. 


par Littr, 


5 


36 


30 


21 


60 


11 


10 


31 


40 


17 


So 


s 


90 


26 






100 






* 0iolved * Mf (HCOi) B . 



Mg MAGNESIUM 954 

SOLUBILITY OP MAGNESIUM CAKBONATE IN WATER CONTAINING CARBON 
UNJDE& HIGH PBESSXJRES AND AT DIFFERENT TEMPERATURES. 

(Hauhnol, 1024.) 

The saturated solutions were prepared in a platinum vessel provided with an 
electrically driven stirrer and contained in an autoclave. After stirring one hour 
and allowing to stand one-half hour the saturated solution was withdrawn through 
a platinum tube and analysed by evaporating and weighing the ignited MgO, 
Equilibrium was approached from above. Magnesium carbonate from different 
sources was used. 

Results at 18. Result* at different temperatures. 

Atmospheres Caw. M * C0 9 pw . . ""* *<*<>> por too fm. mt. sol, at 

Pressure. 100 gms, sat. sol, 

2.0 3.5 

2.5 3.74 

4.0 ,1.28 

lo.o 5.90 

16.0 7oS 

18.0 7-49 

' u 35.o 7.49 

56.o 7.49 

The determinations of Beckurts and of Engle and Vill were made in 1881 
and 1885. 

Electrolytic conductivity results are also given by Haehnel. 

EQUILIBRIUM IN THE SYSTEM MAGNESIUM CAHBONATV, AMMONIUM GA.HBONATE 
AND WATER AT 30 , (UfonnUiie. iro.) 

To a concentrated solution of magnesium bicarbonate containing 20-2$ grams 
Mg (H C0 3 ) a per liter, increasing quantities of ammonia, ammonium bicarbonate 
or of mixtures of the two were added. The solutions wre agitated mechanically 
10 hours per day for 8 days. The eomposition of the solid phase did not change 
but its quantity increased with time. The zones of formation of the several solid 
phases were determined. 



t". 


or c.o, ^r co, 

(Kngtcftml Viu*, tttfekurift). 


.14 atmospheres 
of CO, 
llhrhnel). 


o. 




8.58 


5. 


- 


8i3a 


to. 

3o. 


., - 3.5 7 
..1.58 


7-93 
6.88 


4o. 


. . 1.18 1.37 


6.44 


50. 


. . o.cjS 


6.18 


So. 




5.56 



Mols. pflMW mols. n0.__ a ti 4 Mt. | 

m ~~****~~" ' j hawj( 

.14 



- *! 

M#0 


"""^or"* 


Mam"" -""' 


Flttftft*, Mf O, 


t:0,. 


Kit,. 


O.JGO 


1.487 


1.193 


MgCO.3!l t O o.oi>G 


1,593 


io,3S6 


o.ioS 


a.5o8 


'A . 099 


> 0,091 


"Jui7',i 


i 93% 


0.097 


a. a56 


0.120 


> . oa i 


0,46:1 


j .:i5t 


o.o^i 


0.816 


0.875 


0.019 


o,S8S 


i . .|0a 


o . 02 1 


0.089 


o. 144 


t o.oia 


t . 10<i 


i ,58a 


o.oao 


0.294 


1.168 


n (> 0o8 


0.08 4 


6 . SCi'Ji 


o.o55 


0.95*2 


0.970 


o . 008 


0.<H)'> 


11.029 


0.075 


2.427 


a.VM 


I.t.4 O.O20 


'i'JlO 


3.783 


o.o56 


i . o65 


1.087 


o , oo(i 


0,178 


4.3% 


o.O'iS 


c.3i5 


i.Srf 


*> o . o 1 5 


o . 1 96 


> . ^24 


o.oa4 


3.357 


3 . 269 


> o . o i u 


o. 1 5*4 


H.64 


0.016 


. 623 


1.277 


O , OO I 


0,0 TO 


10.981 


0.008 


3 <7 45 


3.S37 


0,007 


O, MKI 


15,710 


1.1.4 


-MgCO,, 


,(NH 4 ),CO 


,4H,0, 4, 1. 4 4 MgCO,. 


Mg(OH),4H, 


0. 



955 



MAGNESIUM 




was really obtained and furthermore, the accuracy of the analyti 

be trusted since the ratio of total amount of CO in solution, to the mu 

very irregular. The results when plotted directly show great iucontustttncics. 

THE CALCULATED SOLUBILITY OF MgCOi^HbO IN WATER AT 18 IN CONTACT 

WITH AIR CONTAINING PARTIAL PRESSURES OF C() 2 FROM 0.0002 TO o.<xx>5 

ATMOSPHERES. 

(Johnston, 1915.) 

It is shown that if the COa pressure is kept constant at P and the water r\ ,ipn 
rated off so slowly at 18 that equilibrium conditions are continuously mumtainni, 
the following amounts of Mg(OH) or of MgCOi^HsO will be obtained. 



Partial Pressure P 
of COj in Atms. 



o 

O.OOO2O 
O.OOO25 
O.OOO3O 
0.00035 
O.OOO4O 
0,00045 
0.00050 



Total Mg~r-' 
O.OOOI5 
0.01934 



Gmii. per Liter*. 

0.0087 Mg(OH)t 

1.13 

1.29 

x. 45 
i .60 

3-97 
4-05 



''- <" 

truer 

tr.uc 

o.jHCO. 4-.t*ft 
0,34 t'<V' " o 
SOLUTIONS tn> 



:,;','; 



0.02218 
0.02486 
0.02742 
0.02868 

0.02924 

0.02976 4,12 

SOLUBILITY OF MAGNESIUM CARBONATE IN NATURAL WATERS. 

(Wclb, 1915.) 
(In all cases the solutions w