272 PROPERTIES OF ELECTRICALLY CONDUCTING SYSTEMS 



TABLE CVIIL Continued 



Salt added 



HBr 



Equiv. of 

 added salt in 

 1000 g. H 2 



. 0.06817 

 0.4191 

 0.9716 

 1.154 



HI 



KI 



KC1 . 



CuCl 2 

 KNCX 



0.1641 

 0.4462 

 0.4126 

 0.7539 



0.09199 

 0.5401 

 0.6015 

 1.445 



0.0719 

 0.433 

 0.8576 

 1.594 



0.7134 

 2.276 



0.09796 

 0.4755 



Sol. equiv. per 

 1000 g. H 2 



6.974 

 6.696 

 6.262 

 6.132 



6.890 

 6.650 

 6.672 

 6.366 



7.034 

 7.016 

 7.038 

 6.992 



7.016 

 6.950 

 6.882 

 6.764 



6.812 

 6.352 



7.122 



7.406 



at 25 in the presence of different electrolytes. The results are shown 

 graphically in Figure 55. It will be seen from the table and the figure 

 that, up to a concentration of l.ON, the solubility effects are, in general, 

 small. The difference between the effect of salts with and without a com- 

 mon ion is not great. The solubility of strontium chloride remains prac- 

 tically constant on addition of nitric acid, potassium iodide, and stron- 

 tium nitrate. The addition of potassium chloride causes a slight 

 decrease in solubility, while that of sodium nitrate causes a slight in- 

 crease. The greatest decrease in solubility results from the addition of 

 hydrochloric acid, but it is to be noted that hydriodic acid and hydro- 

 bromic acid, which do not have an ion in common with strontium chloride, 

 cause almost as great a solubility depression as does hydrochloric acid. 

 It is clear that, at high concentrations, the solubility effects are not to be 

 ascribed primarily to ionic interaction. The relationships between the 

 solubility effects resemble those obtained in the case of solutions of non- 

 electrolytes in the presence of electrolytes. 



In the Table CIX are given values for the solubility of lanthanum 



