KINETICS OF CERTAIN SILVER SALTS 289 



m <C 0.3 in the case of AgNO 3 , and that we confirmed his 

 result by our own experiments on this and other salts. 

 Consequently the values found for this rate, whenever 

 m = 0.0250.01, can be assumed to hold good for infinite 

 dilutions. The reason becomes apparent when, considering 

 the inactive molecules as stationary, we remember that a 

 molecular concentration 0.01 means a proportion of one sil- 

 ver ion to 5550 molecules of H 2 O. The resistance which 

 such an ion would encounter cannot differ from that of pure 

 water. 



The testing of Kohlrausch's law can now be readily ac- 

 complished by multiplying the limiting value of conductivity 

 into (1 ft), the rate of transference of the positive ion; the 

 product, which represents the molecular velocity of the silver 

 ion, must remain constant for all the monobasic salts. 



TABLE V 

 XX10 8 (1-rc) X(l-n)108 



AgNO 3 1242 0-477 592 



AgCIO, 1172 0-499 585 



AgC10 4 1208 0-486 587 



AgC 2 H 5 SO 4 956 0-615 588 



AgC 10 H 7 SO 3 958 0-614 588 



AgC 6 H 5 SO 3 913 0-653 596 



AgC 9 H u S0 3 842 0.707 595 



AgC 2 H 3 O 2 956 0-624 597 



The velocity of Ag as found in these salts proves to be 

 nearly constant: the deviations from the average 591 X10 8 

 are within the limits of the probable errors of observation, 

 especially as the latter have a cumulative effect. We con- 

 sider this an additional confirmation of the recent electrolytic 

 hypotheses. 



This average, which applies for 25, may be considered the 

 true value for the velocity of the Ag ion, within a few thou- 

 sandths, provided Kohlrausch's determination of the limit of 

 conduction for argentic nitrate contains no important error. 



