CONDUCTION PROCESS IN ELECTROLYTES 45 



TABLE IX. 



VALUES OF K FOR KC1 IN WATER AT 18. 



c= io- 5 io- 4 io- 3 io- 2 lo- 1 i.o 



K=. 00518 .0147 .0474 .1542 .5052 2.14 



It will be observed that in this case the function K decreases enormously 

 with decreasing concentration. Whether the function approaches a finite 

 limit, or whether it approaches a limit zero at low concentrations, cannot 

 be determined with certainty. In general, the stronger the electrolyte, 

 the more does the function K vary with the concentration and the 

 greater is its value at a given concentration. In the case of hydrochloric 

 acid the values of .K at a number of concentrations are as follows: 



TABLE X. 

 VALUES OF K FOR HC1 IN WATER AT 18. 



c= io- 3 io- 2 io- 1 



K = 0.189 0.366 1.11 



If these values are compared with those for potassium chloride, it will be 

 seen that the value of K is considerably greater for hydrochloric acid 

 than it is for potassium chloride. At 0.1 normal the value of K for 

 hydrochloric acid is approximately twice that for potassium chloride. 

 In the more dilute solutions, however, this ratio appears to increase, since 

 in a 0.001 normal solution the value for hydrochloric acid is approxi- 

 mately four times that of potassium chloride. 



In view of the fact that electrolytes of a given type appear to be 

 ionized to practically the same extent in water, it follows that the dis- 

 crepancies found for different electrolytes of the same type will be of 

 the same order of magnitude. 



