40 'PROPERTIES OF ELECTRICALLY CONDUCTING SYSTEMS 



TABLE VI. Continued 

 Electrolyte Method 5X10- 3 10 J 2X10- 2 5X10- 2 10- 1 2X10- 1 5X10- 1 



values of y as determined from freezing point (F) and from conductivity 

 (C) measurements. 



It will be observed that in the case of certain electrolytes the values 

 of y derived by the two methods correspond very closely. This is par- 

 ticularly true of potassium chloride where the two values correspond 

 practically within the limit of experimental error up to concentrations as 

 high as 0.1 normal. In the case of other salts, the divergence at higher 

 concentrations is considerably greater. In general, however, the two 

 values approach each other the more nearly, the lower the concentration 

 of the solution. The correspondence between the two values is closest 

 in the case of the binary salts. The more complex a salt, the greater is, 

 as a rule, the divergence between the two values and the lower the con- 

 centration at which a given divergence appears. 



The cause of the divergence of the ionization values as determined 

 by the two methods is as yet uncertain. It is possible that the ionization 

 is not correctly measured by the conductance ratio. At higher concen- 

 trations, at any rate, it is to be expected that various influences will make 

 themselves felt, such as the effect of viscosity, as a result of which the 

 conductance as measured will not yield a true measure of the ionization. 

 On the other hand, the molecular weight, as determined by osmotic 

 methods, may be expected to be in error, since the laws of dilute solu- 

 tions are assumed in calculating these values. The only assurance we 

 have that the laws of dilute solutions are applicable under given condi- 

 tions is that the results obtained are in agreement with other facts re- 

 lating to these solutions. When a disagreement occurs, therefore, it is 



