WORK OP C. M. STINE. 



41 



ions to show itself in the resulting curve, the other salt in the mixture must have 

 hydrating power and a comparatively small molecular weight; for if the molecular 

 weight is large so much solvent will be displaced when the solutions are made up 

 volume normal that the decreased amount of solvent will obscure any change in 

 hydration due to other causes. Also, the difference in the hydrating power of the 

 ions and molecules should be considerable, in order to overcome the effect of decrease 

 in amount of solvent present with increase in concentration. 



c 



'3 





 o 



S 10 



3 

 i) 

 -Si 



O 



S 



o 



o 



V 







3 



z, 



100- 





o 



.5 1. 



Gram Molecules of Salt per Liter of Solution 

 Fig. 10. 



I. Lithium Bromide Alone. 

 II. Lithium Bromide Mixed with Sodium Bromide. 

 III. Sodium Bromide Alone. 

 IV. Sodium Bromide Mixed with Lithium Bromide. 



r - 



.5 



1. 





3 

 M 



3 

 S 







o 



+1 - 



II 



Gram Molecules of Salt per Liter of Solution 

 Fig. 11. 



Difference between Amount of Water Present as Solvent in Single 

 Solution of Lithium Bromide and in Mixture of Lithium Bromide 

 and Sodium Bromide. 



Difference between Values of M for Lithium Bromide in Single Solu- 

 tion and in Mixture of Lithium Bromide and Sodium Bromide. 



The difference between the amount of water acting as solvent towards each salt in 

 the mixture and in single solution, and the differences between the values of M in the 

 same cases, are given in table 28. A negative value of D m indicates that the number 

 of grams of water eliminated by a salt in a mixture is greater, instead of less, than 

 in single solution. 



Table 28. 



