ELECTROLYTIC SOLUTIONS IN VARIOUS SOLVENTS 47 



sodium iodide in ethyl alcohol, the values of which are given in Table 

 XI: 1 



TABLE XI. 



CONDUCTANCE OF SODIUM IODIDE IN ETHYL ALCOHOL AT 18. 



V 125 250 500 1000 2000 4000 8000 oo 



A 28.6 31.3 33.5 35.2 36.5 37.6 38.3 39.4 



Y 0.726 0.794 0.850 0.894 0.926 0.954 0.972 1.0 



It will be observed that the conductance of solutions in ethyl alcohol 

 increases with decreasing concentration in a manner similar to that 

 of solutions in water. The limiting value of the equivalent conductance, 

 that is the value of A , for a solution of sodium iodide in ethyl alcohol 

 is in the neighborhood of 39.4. It follows, therefore, that the ionization 

 values of solutions in ethyl alcohol are considerably smaller than those 

 of solutions in water. In Figure 3, the ionization of sodium iodide in 

 ethyl alcohol is shown as a function of concentration. In the same figure, 

 the ionization of sodium chloride in water is likewise shown. 



Acetone is another solvent whose solutions resemble those in water 

 in many respects. The conductance of sodium iodide in acetone at 18 

 at a series of concentrations is given in Table XII: 2 



TABLE XII. 



CONDUCTANCE OF SODIUM IODIDE IN ACETONE AT 18. 



V .... 292.6 1030 4083 8874 18660 39700 64827 oo 

 A .... 112.8 131.1 147.7 151.0 154.8 155.2 156.0? 156.0 

 Y 0.723 0.841 0.947 0.968 0.992 0.995 



Here, again, it will be observed that the equivalent conductance rises 

 throughout with decreasing concentration. While the conductance values 

 of acetone solutions are greater than those of solutions in ethyl alcohol, 

 the degree of ionization is very nearly the same in the two solvents. In 

 both ethyl alcohol and acetone the ionization is much lower than it is in 

 water. 



Another typical solvent is found in liquid sulphur dioxide. The con- 

 ductance values of solutions of potassium iodide in sulphur dioxide at 

 33 and at 10 are given in Table XIII: 3 



1 Dutoit and Rappeport, Jour. d. Chim.-Phys. 6, 545 (1908). 

 1 Dutoit and Levrier, Jour. d. Chim.-Phys. 3. 43 (1905), 

 Franklin, J. Pliys. Chem. 15, 675 (1911), 



