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Question

A silver electrode is immersed in saturated Ag2SO4(aq). The potential difference between silver and the standard hydrogen electrode is found to be 0.711 V. Determine Ksp(Ag2SO4).
[Given EAg+/Ag=0.799 V]

Solution
Verified by Toppr

Pt H2H+1MAg2SO4(aq) Saturated |Ag the reaction is
H22H++2e
2Ag++2e2Ag
or, 0.711=0.799+(0.059/2)log[Ag+]2
log(1[Ag+]2)=[0.7990.711]×20.059=3
[Ag+]2=103
[Ag+]=3.2×102
Now, Solubility equilibrium is
Ag2SO42Ag++SO24
Ksp=[Ag+]2[SO24]
=(3.2×102)2(3.2×102)/2
=1.6×105
Ksp[Ag2SO4]=16×105

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