842 REPORTS ON THE STATE OF SCIENCE.— 1912. VI. 
that the order arrived at appeared to indicate some connection between 
this property and the dielectric constants of the liquids. Herz *® 
published data relating to the mutual solubility of water and respectively 
chloroform, carbon bisulphide, ligroin, ether, benzene, amylic alcohol, 
and aniline. 
A communication by Fock **, entitled ‘ Dissociation in Mixed Sait 
Solutions,’ dealt with the solubility of mixed crystals of potassium and 
ammonium chloride and the author showed that, within the limits of 
experimental error, the Distribution Law is obeyed. 
1899 The mutual solubility of methyl-ethyl-ketone and water and 
““* also in the presence of 1.5 per cent. alcohol was studied 
experimentally by Bruni.** He also traced the freezing-point curve for 
that system and found that it had no point in common with the liquid- 
solubility curve. 
Lotmar *° found that p-nitrophenol towards the systems water- 
benzene, water-chloroform, &c., exhibits a partition relationship which 
is almost independent of temperature, and which is different from the 
relationship which exists between its solubilities in the separate solvents. 
When aniline and water are mixed together Aignan and Dugas *° 
found that there is no change of volume consequent on the reciprocal 
solubility of the liquids, although in the case of amylic alcohol a volume 
change was observed. 
1900 Newth 7° found that if ordinary strong aqueous ammonia and 
* asaturated solution of potassium carbonate be shaken together two 
layers are formed. Calling the original solutions A and B, the two layers 
are saturated solutions of A in B, and Bin A respectively. It was found 
that by adding suitable quantities of water, mixtures could be obtained 
which were critical for any desired temperature. 
Van der Lee 7° investigated the influence of pressure on the mutual 
solubility of water and phenol. The results found showed that increased 
pressure raises the critical point in accordance with the requirements of 
Van der Waal’s theorem when applied to solutions. Dawson and 
1901 McCrae *? examined the distribution of ammonia between water 
* and chloroform at 15° and 30° C. For solutions less than 0.5 N, 
the distribution coefficient 
conc. of NH, in water 
cone. of NH; in chloroform 
is constant at constant temperature, but, for solutions of greater con- 
centration it falls. If copper sulphate be dissolved in the water, the 
coefficient rises owing to the ‘ fixation ’ of the ammonia by the copper 
1909, Salt. Extending this work to the investigation of the distribution 
“~"* of acetic acid between water and chloroform Dawson and Grant 1*° 
found that the ratio varies greatly with.concentration, but is little 
affected by the presence of sodium acetate or tartaric acid. 
In the course of experiments on the distribution of iodine between 
water and a mixture of two organic solvents, Dawson 1?? found the 
solvent power of such a mixture to be generally less than that which is 
calculated from a knowledge of the solvent powers of the liquids on the 
assumption that they form a simple mixture. In the case, however, of 
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