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Question

A solution of AgNO3 was electrolysed between silver electrodes. Before electrolysis, 10 g of solution contained 0.01788 g of AgNO3. After the experiment, 20.09 g of the anodic solution contained 0.06227 g of AgNO3. At the same time, 0.009479 g of Cu was deposited in the copper coulometer placed in series. Calculate transport no. of Ag+. Write answer to the nearest integer after multiplying transport number calculated with 10.

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Solution

After electrolysis:
20.09g of anodic solution contained 0.06227 g of AgNO3
Mass of water in solution =20.090.06227=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 =100.01788=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
=0.00036630.000211
=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
=0.00029810.0001553
=0.0001428 equivalent of Ag+
Transport no. of tAg+=Eq. ofAg+lost in anodic cellEq. ofCu+deposited in coulometer
=0.00014280.0002981
tAg+=0.4795
Now, tAg++lNO3=1
tNO3=10.4792=0.5215

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