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

The Mn^(3+) ion is unstable in solution and undergoes disproportionati

1.	The Mn^(3+) ion is unstable in solution and undergoes disproportionation to give Mn^(2+),MnO_(2),andH^(+) ion. Write a balanced ionic equation for the reaction.
Answer» SOLUTION :`Mn_((aq))^(+3)toMn_((aq))^(+2)+MnO_(2(s))+H_((aq))^(+)` HALF reaction … O.H.R. : `Mn_((aq))^(+3)toMnO_(2(s))` R.H.R. : `Mn_((aq))^(+3)toMn_((aq))^(+2)` Balancing the reaction on adding `e^(-)` O.H.R. : `Mn_((aq))^(+3)toMnO_(2(s))+e^(-)` R.H.R. : `Mn_((aq))^(+3)+e^(-)toMn_((aq))^(+2)` ADDITION of `H_(2)O` for the balancing of hydrogen and OXYGEN. O.H.R. : `Mn_((aq))^(+3)+2H_(2)OtoMnO_(2(s))+4H_((aq))^(+)+e^(-)` R.H.R. : `Mn_((aq))^(+3)+e^(-)toMn_((aq))^(+2)` Now on addition of O.H.R. and R.H.R. `2Mn_((aq))^(+3)+2H_(2)O_((L))toMnO_(2(s))+2Mn_((aq))^(+2)+4H_((aq))^(+)`