0.5L OF A 0.6M SnSO4 SOLUTION IS ELECTROLYSED FOR A PERIOD OF 30 MINUTES USING A CURRENT OF 4.6A . IF INERT ELECTRODES ARE USED WHAT IS THE FINAL CONCENTRATION OF Sn2+ REMAINING IN SOLUTION?

Faraday's laws can be summarized by

m=(Q/F)(M/Z)

where:

mis the mass of the substance liberated at an electrode in grams
Qis the total electric charge passed through the substance
F= 96485 C mol−1is theFaraday constant
Mis the molar mass of the substance
zis the valency number ofionsof the substance (electrons transferred per ion).

MOLE of SnSO4=(4.6*30*60)/(96500*2)
=.0429 mole
mole of SnSO4 taken=.5*.6=.3 mole
mole left=.3-.0429=.257 mole
concentration=.257/.5=.514 M