Kd for dissociation of [Ag(NH3)2]+ into Ag+ and NH3 is 6×10−8. Calculate E∘ for the following half reaction; Ag(NH3)+2+e−→Ag+2NH3 Given Ag++e−→Ag,E∘=0.799V
A
0.456V
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B
0.373V
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C
0.893V
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D
0.593V
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Solution
The correct option is B0.373V Ag→Ag++e−ERP=0.799V Ag(NH3)+2+e→Ag+2NH3ERP=? Ag(NH3)+2⇌Ag++2NH3 Ecell=E∘cell+0.05911log10[Ag(NH3)+2][Ag+][NH3]2 0=E∘cell+0.05911log(6×10−8)⇒E∘cell=−0.426 E∘cell=E∘C−E∘A −0.426=E∘C−0.799⇒E∘C=0.373V