At what \(\mathrm{pH}\), given half cell \(\mathrm{MnO}_{4}^{-}(0.1 \mathrm{~M}) \mid \mathrm{Mn}^{2+}(0.001 \mathrm{~M}…

At what \(\mathrm{pH}\), given half cell \(\mathrm{MnO}_{4}^{-}(0.1 \mathrm{~M}) \mid \mathrm{Mn}^{2+}(0.001 \mathrm{~M})\) will have electrode potential of \(1.282 \mathrm{~V}\) ?

(Nearest Integer)

Given: \(\mathrm{E}_{\mathrm{MnO}_{4}^{-} / \mathrm{Mn}^{2+}}^{\circ}=1.54 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{~V}\)

[JEE Main 2023, 1 Feb (Shift 1)]