V.c. il. ON SOLUBILITY. 825 
Dawson and Goodson*** continued their work on the solubility of 
iodine in salt solutions and published further results showing that the 
iodides of sodium, rubidium, cesium, lithium, strontium, barium, and 
tetramethylammonium all behave like potassium iodide in so far as 
they increase the solubility of iodine in nitrobenzene. 
Euler *'® studied the lowering of solubility of aniline in water 
occasioned by certain chlorides and by sodium and potassium hydroxide. 
Later in the same year?! he compared the parallel effect of different 
electrolytes in lowering the solubility of hydrogen, nitrous oxide, and 
ethylic acetate in water. He concluded that the equivalent lowering of 
solubility is an additive property of the two dissolved substances and 
he showed that if 7], and 1 represent the solubilities in water and 
solution respectively and ¢ the concentration of salt, then, 
l, oa = a constant. 
In a later communication,?"! in which he included a general sum- 
mary of his own results and those of many other workers showing 
the influence of electrolytes on the solubility of non-electrolytes, this 
author suggested the expression a ° = as being independent of the 
concentration. * 
The solubility of gases in aqueous solutions of electrolytes has also 
been studied by Knopp 1°* and by Geffcken.2° The latter connected 
the influence of electrolytes on the solubility of gases with their effect 
on the internal pressure of the solution. 
The interesting observation was made by Herz and Knoch 2° that 
potassium permanganate and sodium chloride are more soluble in water 
containing acetone than in pure water, although these substances by 
themselves are almost insoluble in pure acetone. 
1905 Continuing this work with potassium bromide and am- 
" monium chloride dissolved in aqueous acetone, these authors 251 
observed a behaviour similar to that previously found with sodium 
chloride, and the relationship ve =constant, suggested by Bodlander, 
was found to be true in these cases. With mercuric iodide dissolved in 
aqueous alcohol, such relationship was not found to be true. Experi- 
ments were made also with various salts dissolved in aqueous solutions 
of glycerol and, in a subsequent publication, these authors 2°? recorded 
their observations of an increased solubility of calcium hydrate being 
occasioned by increasing the amount of glycerol present in the solvent. 
The solubility relationship, in the case of calcium hydrate and aqueous 
glycerol, they expressed in the form of a mathematical equation. 
Fleckenstein 743 observed that whilst the presence of ethylic alcohol 
diminishes the solubility of ammonium nitrate in water the addition of 
methylic alcohol to the water increases the solubility of that salt. He 
*In this expression /=solub. in aqueous solution; J, = solub. in water ; 
n=grammes of substance per litre of aqueous solution ; y=degree of dissociation of 
substance, 
