At what pH, given half cell $\mathrm{MnO_{4}^{-}(0.1~M)~|~Mn^{2+}(0.001~M)}$ will have electrode potential of 1.282 V? ___________ (Nearest Integer) Given $\mathrm{E_{MnO_4^ - |M{n^{2 + }}}^o}=1.54~\mathrm{V},\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.059\mathrm{V}$

Question

At what pH, given half cell $\mathrm{MnO_{4}^{-}(0.1~M)~|~Mn^{2+}(0.001~M)}$ will have electrode potential of 1.282 V? ___________ (Nearest Integer)

Given $\mathrm{E_{MnO_4^ - |M{n^{2 + }}}^o}=1.54~\mathrm{V},\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.059\mathrm{V}$

Correct Answer

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