Question
Permanganate ion $\left( MnO _4^{-}\right)$gives different reduction products at different concentration of hydrogen ions, write their equations.

Answer

The products formed in the reduction reaction of permanganate ion depend on the concentration of hydrogen ion. The reactions occurring at different concentration of $H ^{+}$ are as follows:
$
\begin{aligned}
MnO_{+7}^{-}+e^{-} & \rightarrow \underset{+6}{MnO_4^{2-}} \\
MnO_4^{-}+4 H^{+}+3 e^{-} & \rightarrow \underset{+4}{MnO_2}+2 H_2 O \\
MnO_4^{-}+8 H^{+}+5 e^{-} & \rightarrow Mn^{2+}+4 H_2 O
\end{aligned}
$
Water should be oxidized by permanganate ion at $\left[ H ^{+}\right]$ $=1$ but this reaction happens very slowly but in this. The rate of reaction increases by using $Mn ^{2+}$ ion as a catalyst or by increasing the temperature.

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