CONDUCTION PROCESS IN ELECTROLYTES 43 



of a binary electrolyte. In general, to test the applicability of this 

 equation, the value of A must first be determined by some method of 

 extrapolation, after which the constancy of the function K may be 

 determined by substituting in the above equation. In Table VII 31 are 



TABLE VII. 

 VALUES OF K FOR ACETIC Aero IN WATER AT 25. 



V A K X 100 



0.989 1.443 0.001405 



1.977 2.211 0.001652 



3.954 3.221 0.001759 



7.908 4.618 0.001814 



15.816 6.561 0.001841 



31.63 9.260 0.001846 



63.26 13.03 0.001846 



126.52 ' 18.30 0.001847 



253.04 25.60 0.001843 



506.1 35.67 0.001841 



1012.2 49.50 0.001844 



2024.4 68.22 0.001853 



oo 387.9 



given values for the conductance of acetic acid in water at 25 at a 

 series of concentrations. In this table, V denotes the dilution in liters 

 per equivalent, A the equivalent conductance and K the ionization con- 

 stant, calculated according to Equation 7. 



It will be seen that at higher concentrations, down to about 0.1 nor- 

 mal, there is a marked change in the value of the function K, but at 

 concentrations below 0.1 normal the function K remains constant, prac- 

 tically within the limits of experimental error. 31 * At the highest dilution 

 in the table the function K shows a slight increase, which is probably 

 due to a discrepancy between the experimental values and the assumed 

 value of A . In general, the weaker the acid, the greater the range of 

 concentration over which the function K remains constant. In other 

 words, the concentration, at which the function K varies measurably 

 from constancy, increases as the strength of the acid increases. In Table 

 VIII 32 are given values of the equivalent conductance and the ionization 

 constant of trichlorobutyric acid at a series of concentrations. It will be 



11 Kendall, Med. Veten. Aka4. Nobelinstitut 2, No. 38, p. 1 (1913). 



ia The decrease in the value of K at higher concentrations is in part, if not largely, 

 due to the increasing viscosity of the solution. Compare Washburn, "Principles of Physi- 

 cal Chemistry," 2nd Ed., p. 340. 



a Kendall, loc. cit. 



