A silver electrode is immersed in saturated Ag2SO4(aq). The potential difference between silver and the standard hydrogen electrode is found to be 0.711V. Determine Ksp(Ag2SO4).
[Given E∘Ag+/Ag=0.799V]
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PtH2∣∣H+1M∣∣Ag2SO4(aq) Saturated |Agthe reaction is
H2⟶2H++2e−
2Ag++2e−⟶2Ag
or, 0.711=0.799+(0.059/2)log[Ag+]2
log(1[Ag+]2)=[0.799−0.711]×20.059=3
[Ag+]2=10−3
[Ag+]=3.2×10−2
Now, Solubility equilibrium is
Ag2SO4⟷2Ag++SO2−4
Ksp=[Ag+]2[SO2−4]
=(3.2×10−2)2(3.2×10−2)/2
=1.6×10−5
Ksp[Ag2SO4]=16×10−5
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