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Nernst Equation

For which of ...

Question

For which of the following, E $_{O P}$ will vary with pH of the solution?

M n^{2 +} / M n O_{4}^{-}

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C r^{3 +} / C r O_{4}^{2 -}

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N i / N i^{2 +}

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N O_{2} / N O_{3}^{-}

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Solution

The correct options are
A $M n^{2 +} / M n O_{4}^{-}$
B $C r^{3 +} / C r O_{4}^{2 -}$
D $N O_{2} / N O_{3}^{-}$
$E_{O P}$ will vary with the pH of solution for $M n^{2 +} / M n O_{4}^{-}, C r^{3 +} / C r O_{4}^{2 -} a n d N O_{2} / N O_{3}^{-}$ . This is because in the net electrode reaction, the concentrations of various species depends on the hydrogen in concentration.
The pH will not vary for the $N i / N i^{2 +}$ . This is because in the net electrode reaction, the concentrations of various species does not depends on the hydrogen in concentration.

Suggest Corrections

Similar questions

E_{C r^{3 +} / C r}^{\circ} = - 0.74 V; E_{M n O_{4}^{-} / M n^{2 +}}^{\circ} = + 1.51 V

E_{C r_{2} O_{7}^{2 -} / C r^{3 +}}^{\circ} = + 1.33 V; E_{C l / C l^{-}}^{\circ} = + 1.36 V

M n O_{4}^{-}

N O_{2}^{-}

N O_{3}^{-}

N O_{2}^{-}

1

M n O_{4}^{-} ?

△ G^{\circ}

M n O_{4}^{-} | M n O_{2}

x F

x

E_{M n O_{4}^{-} | M n^{2 +}}^{\circ} = 1.5 V; E_{M n O_{2} | M n^{2 +}}^{\circ} = 1.25 V

C r_{2} O_{7}^{2 -} + H^{+} + I^{-} \to C r^{3 +} + I_{2} + H_{2} O

C r_{2} O_{7}^{2 -} + F e_{2}^{+} + H^{+} \to C r^{3 +} + F e^{3 +} + H_{2} O

M n O^{4 -} + S O_{3}^{2 -} + H^{+} \to M n^{2 +} + S O_{4}^{2 -} + H_{2} O

M n O^{4 -} + H^{+} + B r^{-} \to M n^{2 +} + B r_{2} + H_{2} O

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