The `Mn^(3+)` ion is unstable in solution and undergoes disproportionation to give `Mn^(2+)` , `MnO_(2)`, and `H^(+)` ion. Write a balanced inoic equation for the reaction .

Explanation

`Mn^(3+)` is unstable in aqueous medium and undergoes disproportionation reactions formaing `Mn^(2+) ,MnO_(2)` and `H^(+)` So the reaction is -
`Mn^(3+)(aq)toMn_(2+)(aq)+MnO_(2)(s)+H^(+(aq)`
Here the oxidation reaction is -
`Mn^(3+)(aq)+2H_(2)O(l)toMnO_(2)(s)+4H^(+)(aq)+e`
and the reduction reaction is-
`Mn^(3+)(aq)+etoMn^(2+)(aq)`
Adding equation (1) and equation (2) we have
`2Mn^(3+)(aq)+2H_(2)O(l)toMnO_(2)(s)+Mn^(2+)(aq) +4H^(+)(aq)`
This balanced equation for the disproprotionation reaction that `MN^(3+)` ion undergoes in aqueous medium .