After electrolysis:
∵20.09g of anodic solution contained 0.06227 g of AgNO3
∴ Mass of water in solution =20.09−0.06227=20.02773g
Thus, 20.02773gH2O has 0.06277 g AgNO3
=0.06227170equivalentAgNO3
=0.0003663equivalentAgNO3 or Ag+
Before Electrolysis:
∵10.0g of solution contained 0.01788 g AgNO3
∴ Mass of water in solution =10−0.01788=9.98212g
Thus, 9.98212 g water has =0.01788 gAgNO3
=0.01788170 eq. AgNO3
∴20.02773g water has =0.01788×20.02773170×9.98212 eq. AgNO3
=0.000211 equivalent of AgNO3 or Ag+
Thus, increase in concentration of Ag+ during electrolysis
=0.0003663−0.000211
=0.0001553 equivalent
Also, Mass of Cu deposited in coulometer =0.009479 g
∴ Equivalent of Cu deposited in coulometer =0.00947931.8
∴ Equivalent of Cu deposited or actual increase around anodic solution
=0.0002981 eq.
(Since, equal equivalents are discharged at either electrode)
Since, Ag+ had migrated from anode, which brings a fall in concentration around anode but due to attacked electrodes, (i.e., Ag in AgNO3), apparent increase is noticed.
Thus, fall in concentration of Ag+ around anode
= Actual increase which would have occur around anode - Apparent increase in Ag+ around anode
=0.0002981−0.0001553
=0.0001428 equivalent of Ag+
∴ Transport no. of tAg+=Eq. ofAg+lost in anodic cellEq. ofCu+deposited in coulometer
=0.00014280.0002981
tAg+=0.479≈5
Now, tAg++lNO−3=1
∴tNO−3=1−0.4792=0.521≈5