ELECTROLYTIC SOLUTIONS IN VARIOUS SOLVENTS 59 



TABLE XXII. 

 VALUES OF K AND A FOR DIFFERENT ELECTROLYTES IN NH 3 AT 33. 



Salt WK A 



NaNH 2 0.056 263 



KNH 2 1.20 301 



Agl 2.90 287 



NH 4 C1 12.0 310 



NaCl 14.5 309 



KN0 3 15.5 339 



KBr 21.0 340 



T1N0 3 21.0 323 



NaBr0 3 23.0 378 



NaN0 3 23.0 301 



NH 4 Br 23.0 303 



LiN0 3 26.0 283 



NaBr 27.0 302 



Nal 28.0 301 



AgN0 3 28.0 287 



NH 4 N0 3 28.0 302 



KI 42.0 339 



ferences in the ionization values of the different electrolytes are neces- 

 sarily very small. Nevertheless, we must conclude that the ionization 

 values of typical salts in water are much more nearly the^same in that 

 solvent than they are in ammonia or in any other solvent for which 

 reliable data are available. The order of the ionization constants does not 

 appear to bear any relation to the constitution of the electrolytes. So 

 ammonium chloride has an ionization constant of 12 X 10"* and am- 

 monium nitrate of 28 X 10~ 4 , while silver iodide has an ionization con- 

 stant of 2.9 X 10"* and silver nitrate 28 X 10"*. Sodium nitrate has a 

 greater ionization constant than potassium nitrate, while sodium iodide 

 has a smaller ionization constant than potassium iodide. 



The constants for sodium and potassium amides are of interest owing 

 to the fact that these substances are bases in liquid ammonia solution. 

 Apparently these substances are relatively weak bases when compared 

 with the typical salts in ammonia or when compared with corresponding 

 bases in water. Indeed, it is apparent that all electrolytes in ammonia 

 solution have comparatively small ionization constants. For example, 

 the ionization constant of acetic acid in water is 0.182 X 10"*. The 

 ionization constant of this acid, therefore, is approximately three times 

 that of sodium amide and 1/7 that of potassium amide. 



The ionization constants for a number of organic electrolytes in liquid 



