830 REPORTS ON THE STATE OF SCIENCE.—1912. V.c. iii. 
solved in water was found to be parallel to the behaviour of hydrogen 
chloride. Glucose increases the solubility of chlorides. 
The solubility of carbon dioxide in aqueous solutions of various non- 
electrolytes was experimentally studied by Usher.***4 “When the solu- 
bility was calculated on a weight-normal basis he found that eleven out 
of the fifteen substances added to the water rendered the solution 
a better solvent for carbon dioxide—the substances which decreased 
the solubility being sucrose, glucose, mannitol and glycine. The be- 
haviour of n-propylic alcohol is of particular interest, inasmuch as the 
presence of one-half a molecular proportion of it added to 1,000 grammes 
of water causes the solution of 24 ccms. of carbon dioxide over and 
above that which normally dissolves in the same weight of water. 
Drucker and Moles **? determined the solubility of hydrogen and 
nitrogen in various mixtures of iso-butyric acid and water. They 
found with these mixtures that, even at the critical solution point, the 
gases obeyed Henry’s law. 
In the next year, Sidgwick and others *°° examined the effect pro- 
duced upon the solubility of aniline in water at different temperatures 
by the addition of aniline hydrochloride to the mixture. Very curious . 
results were obtained, which were attributed to the great change in the 
distribution coefficient of the hydrochloride between aniline and water 
occasioned by varying the concentration of the salt. 
V. C.—Influence of other Substances. 
(iii). Electrolytes influenced by Electrolytes. 
1896 Kiister '* published a criticism of the work of Fresenius and 
* Heinz which dealt with the solubility of barium sulphate in 
solutions of various salts and acids, and he expressed the opinion that 
their results are only of qualitative value. The solubility in question 
was considered by Kiister to be dependent upon the mass law and upon 
the reciprocal influence of the electrolytes in solution. 
1897 A particular case is afforded of the mutual influence of salts 
’ in solution where double-salts are formed, and such conditions 
were investigated by Rimbach'’ who compared the solubility of a 
number of double cadmium chlorides with those of their constituents. 
At 0° G. the solubility of the double-salt was found to lie between the 
solubilities of the constituents; but the temperature coefficient is much ~ 
greater for the double-salt than for the constituent substances. 
The problem presented by double-salt formation was also con- 
sidered by Hoitsema *° in a paper dealing with aqueous solutions of two 
salts with one common ‘ion.’ Considering the effect of double-salt 
formation in which the resultant combination dissociates into the two 
original salts, this author concluded that the addition of one salt must 
at first cause a decreased and then an increased solubility of the other 
salt. In those cases where complex salts are formed which dissociate 
into fresh ‘ ions,’ the solubility at first becomes increased and then de- 
creased on the addition of a second salt. 
Ditte 2° found that the solubility of chlorides, bromides, and iodides 
of the alkali metals is diminished considerably by the presence of the 
hydroxides of these metals in the solution. 
