ON SOLUBILITY * 439 



1S56. Kremers 21 , 22 continued work on the solubility of salts. In 



1857 ^ e fo ' lowm S }' ear a memoir was published by Abascheff ~ 7 on the 



solubility of one liquid in another; he was probably the first to 



ascertain that liquids only partly miscible at ordinary temperatures are 



often completely miscible at higher temperatures. 



o- Sims 31 examined the absorption of ammonia in water (vide 



Section V. B) at various temperatures, and found that with rising 



temperature the absorption more nearly approached the requirements 



of Henry's law. Contrary to the conclusion of Schonfield,* he also 



showed that sulphur dioxide only obeyed this law above 4(P. Following 



the systematic study of solubility of salts in water carried out by 



„„. Alluard 30 and by Mulder, 37 the above observations made by Sims 



were supported by the results obtained by Walls. 36 A general 



1865. expression connecting solubility and temperature was proposed 



1S69 ky Nordenslcjold,' 16 who observed how the solubility generally 



increased disproportionately with the temperature; increasing 



more rapidly. 



Among other complicated relations between solubility and tempera- 

 Q „ r ture AlexejefJ B4 found the solubility of amylic alcohol in water 

 decreased with rise of temperature, while that of water in amylic 

 alcohol increased with rise of temperature. 



Setschenoff ir ' A reinvestigated the solubility of gases in liquids, and 

 obtained results which were not in agreement with those recorded by 

 -oon Bunsen ; additional doubt was thrown upon those long recognised 



values by Naccari and Pagliani. 83 

 18S1 Previous to the work of Precht and Wittjen ss the solubility uf 



salt mixtures had been studied at only a small range of tempera- 

 ture.! These investigators found, among other interesting points, that 

 between 10° and 100° C. the solubility of KC1 in presence of K 2 S0 4 in 

 water was practically the same as in pure water. In dilute solutions of 

 NaCl the solubility of BaCl 2 , although somewhat depressed, increased 

 with rise of temperature at almost the same rate as it does in water only. 

 -1009 Their continuation of this work, 91 using mixtures of salts such as 

 l ~ 1 " ' occasion double salt formation, gave results difficult to interpret. 

 Determinations of the solubility of calcium butyrate in water at 

 various temperatures were made by Hecht.* 2 His results showed a 

 solubility decrease as the temperature rose from 0° to C5°, between 

 05° and 80° the solubility was constant, and from 80° to 100° it slowly 

 increased with rise of temperature. 



Goodwin 93 studied the influence of certain metallic chlorides on the 

 solubility of chlorine at various temperatures. Wroblewshi 9>1 measured 

 the absorption of gases by liquids at high temperatures. Later on 

 1Rfi „ de Copped, 97 who experimented on the lines of Gay-Lussac, but 

 employed more delicate means of maintaining a constant tem- 

 perature, was led to the conclusion that when solubility values are 



ammonia in water (Ann. Ch. Pharm., 1856, 99, 129, and also by others, vide footnote 

 Section V. A, 1890). * Ann., 1854, 95, 1. 



t 1879. J. Schonach '" studied solution of NaCl with KC1 at temperatures from 

 0° to 100°, but could obtain no simple mathematical relationship. Vide Section 

 V. C (iii). 



