The Mn^(3+) ion is unstable in solution and undergoes disproportionation to give Mn^(2+) , MnO_(2) and H^(+) 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) and H^(+) ion. Write a balanced ionic equation for the reaction.
Answer» Solution :The skeletal equation is: `Mn_(aq)^(3+) RARR Mn_(aq)^(2+) + MnO_(2_((s))) + H_((aq))^(+)` Oxidation HALF equation: `Mn_((aq))^(3+) rarrMnO_(2_((s)))` Balance O.N. by adding electrons, `Mn_((aq))^(3+) rarrMnO_(2((s))) + e^(-)` Balance charge by adding `4H^(+)`ions Balance O atoms by adding `2H_(2)O` `Mn_((aq))^(3+)+2H_(2)OrarrMnO_(2((s)))+4H_((aq))^(+)+e^(-)` Balance O atoms by adding `2H_(2)O` `Mn_((aq))^(3+)+2H_(2)O_((l))rarrMnO_(2((s)))+4H_((aq))^(+)+e^(-)`.......................(1) Reduction half equation: `Mn^(3+)rarrMn^(2+)` Balance O.N. by adding electrons: ` Mn_((aq))^(3+) + e^(-) rarr Mn_((aq))^(2+)` ..............(2) Adding Equation (1) and (2), the balanced equation for the disproportionation reaction is `2Mn_((aq))^(3+)+2H_(2)O_((l)) rarr MnO_(2_((s)))+Mn_((aq))^(2+)+4H_((aq))^(+)`