After electrolysis:∵20.09g of anodic solution CONTAINED 0.06227 g of AgNO 3 ∴ Mass of water in solution =20.09−0.06227=20.02773gThus, 20.02773gH 2 O has 0.06277 g AgNO 3 = 1700.06227 equivalentAgNO 3 =0.0003663equivalentAgNO 3 or Ag + Before Electrolysis:∵10.0g of solution contained 0.01788 g AgNO 3 ∴ Mass of water in solution =10−0.01788=9.98212gThus, 9.98212 g water has =0.01788 gAgNO 3 = 1700.01788 eq. AgNO 3 ∴20.02773g water has = 170×9.982120.01788×20.02773 eq. AgNO 3 =0.000211 equivalent of AgNO 3 or Ag + THUS, increase in concentration of Ag + during electrolysis=0.0003663−0.000211=0.0001553 equivalentAlso, Mass of Cu deposited in coulometer =0.009479 g∴ Equivalent of Cu deposited in coulometer = 31.80.009479 ∴ 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 AgNO 3 ), 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 t Ag + = Eq. ofCu + deposited in coulometerEq. ofAg + lost in anodic cell = 0.00029810.0001428 t Ag + =0.479≈5Now, t Ag + +l NO 3− =1∴t NO 3− =1−0.4792=0.521≈5