ELECTROLYTIC SOLUTIONS IN VARIOUS SOLVENTS 63 



TABLE XXV. Continued. 

 Solute 10 4 K A 



NH 4 I 15.0 159 



KSCN 31.0 169 



LiSCN 18.0 167 



NH 4 SCN 8.3 172 



KBr 16.0 156 



NaBr 13.0 156 



LiBr 5.7 154 



NH 4 Br 2.3 159 



LiN0 3 2.6 125 



AgN0 3 0.28 100 



LiCl 0.94 154 



From an examination of this table it is obvious that the ionization con- 

 stants of typical salts in acetone vary within very wide limits. So, the 

 ionization constant for silver nitrate is 0.28 X 10'*, whereas that for 

 potassium iodide is 51.0 X 10"*. More remarkable still is the regularity 

 in the variation of the constants as a function of the constitution of the 

 electrolyte. The ionization constants of the iodides diminish in the order 

 potassium, sodium, lithium, ammonium. The same order holds in the 

 case of all other salts, namely the sulfocyanates, bromides, and nitrates. 

 On the other hand, the ionization constants of salts with a common posi- 

 tive ion vary in the order: iodides, sulfocyanates, bromides, nitrates, 

 chlorides. This order holds true in every case. It appears, therefore, 

 that the ionization constant K is an additive function of the constituent 

 ions of the electrolytes. This is the only solvent for which such a rela- 

 tion appears to hold true. What the significance of this may be is at 

 present uncertain. It is important, however, to observe that the ioniza- 

 tion of different typical salts in acetone varies within extremely wide 

 limits. The similarity in the behavior of strong electrolytes in aqueous 

 solutions, as regards their ionization, is therefore not to be considered as 

 a property which may be ascribed primarily to the electrolytes them- 

 selves, but rather one in which the solvent itself appears as the chief 

 factor. 



3. Comparison of the Ion Conductances in Different Solvents. If 

 the values of A are known and if the transference numbers of the 

 electrolytes are known, then the values of the ion conductances may be 

 determined. However, before proceeding to a comparison of the values 

 of the ion conductances in different solvents, it will be well to point out 

 that the value of A is dependent upon the form of the extrapolation 

 function which must be assumed. Only in the case of solutions which 



