18 



WORK OF C. M. STINE. 

 Table 5. Calcium and Potassium Chlorides in the Mixture. 



Calcium chloride in the mixture. 



m 



m c 



a 



1.0CaCIH-0.9KCl... 

 1.4CaCl 2 +1.3KCl... 

 1.8CaCl 2 +1.7KCI... 

 2.2CaCl 2 +2.1KCl... 

 2.7 CaCl 2 +2.59 KC1 . 

 3.1CaCl 2 +2.59KCl.. 

 3.51 CaCl 2 +2.59KCl. 



0.5 



0.7 



0.9 



1.1 



1.35 



1.55 



1.7553 



0.573 

 0.529 

 0.491 

 0.452 

 0.404 

 0.375 

 0.355 



3.992 

 3.829 

 3.687 

 3.541 

 3.362 

 3.256 

 3.179 



2.034 

 2.769 

 3.464 

 4.126 

 4.880 

 5.462 

 6.084 



Potassium chloride in the mixture. 



m 



m c 



a, 



Wh*) 



Correction, 

 per cent. 



U 



1.0CaCl 2 +0.9KCl.. 

 1.4CaCl 2 +1.3 KC1.. 

 1.8CaCl 2 +1.7KCL. 

 2.2CaCl 2 +2.1 KC1.. 

 2.7CaCl 2 +2.59KCl. 

 3.1CaCl 2 +2.59KCl. 

 3.5lCaCl 2 +2.59KCl 



0.45 



0.65 



0.85 



1.05 



1.2972 



1.2972 



1.2972 



0.766 

 0.748 

 0.716 

 0.681 

 0.649 

 0.624 

 0.581 



1.478 

 2.113 

 2.712 

 3.283 

 3.068 

 3.021 

 2.941 



753.7 

 655.9 

 608.2 

 538.5 

 464.7 

 408.0 

 340.5 



24.6 

 34.4 

 39.2 

 46.2 

 53.5 

 59.2 

 66.0 



1.961 

 3.222 

 4.454 

 6.097 

 8.564 

 9.605 

 11.20 



a is the dissociation of the calcium chloride in the mixture. L is the freezing- 

 point lowering calculated from the formula (1.86 X2a) + 1.86. I is the freezing- 

 point lowering, corrected to 1,000 grams of solvent, which the salt would give if there 

 were no hydration. 



ai is the dissociation of the potassium chloride in the mixture ; A is the freezing- 

 point lowering deduced from [(1.86Xa) + 1.86]w c ; Wh& is the weight of water 

 acting as solvent towards the potassium chloride, deduced from L : L : : X: 1,000, 

 which gives the amount of water taken up by the calcium chloride in the formation 

 of hydrates when it alone is present in solution, and from the weight-normal correc- 

 tion for the mixture; I\ is the theoretical lowering which the potassium chloride 

 would give if the calcium chloride formed the same hydrates in the mixture that it 

 forms when alone in solution. 



LOWERING DUE TO HYDRATION. 



In table 6, A c is the lowering found experimentally for the mixture. T c = sum of 

 J and 1 1 in table 5. Diff c = A 7 e = lowering due to hydration. A = lowering found 

 experimentally for calcium chloride, corrected to 1,000 grams of solvent. I is the 

 lowering the calcium chloride should have given in 1,000 grams of solvent if there 

 were no hydration. Evidently, Diff c and Diff. should be identical if there were no 

 change in hydration; such is not the case. Therefore, the basis assumed for the 

 calculation of I for potassium chloride in the mixture is incorrect, as it depends 

 upon a knowledge of the amount of water eliminated from the sphere of action as 

 solvent by the hydration of the calcium chloride. It therefore becomes necessary 

 to derive a formula for the calculation of the hydration of the calcium chloride in the 

 mixture. 



