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Question
\[\ce{MnO^{2-}4}\] undergoes disproportionation reaction in acidic medium but \[\ce{MnO^{-}4}\] does not. Give reason.
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Solution
In \[\ce{MnO^{2-}4}\], Mn is in highest oxidation state that is +7 hence here manganese cannot undergo oxidation that is why disproportionate is not possible whereas in \[\ce{MnO^{2-}4}\] manganese is in +6 oxidation state which can be oxidized as well as reduced.
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