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The Mn3+ Ion is Unstable in Solution and Undergoes Disproportionation to Give Mn2+, Mno2, and H+ Ion. Write a Balanced Ionic Equation for the Reaction. - Chemistry

The Mn3+ ion is unstable in solution and undergoes disproportionation to give Mn2+, MnO2, and H+ ion. Write a balanced ionic equation for the reaction.

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Solution

The given reaction can be represented as:

`Mn_(aq)^(3+) -> Mn_(aq)^(2+) + MnO_(2(s)) + H_(aq)^+`

The oxidation half-equation is:

The oxidation number is balanced by adding one electron as:

`Mn_((aq))^(3+) -> MnO_(2(s)) + 4H_((aq))^  + e^(-)`

The O atoms and H+ ions are balanced by adding 2H2O molecules as:

`Mn_(aq)^(3+) -> Mn_(aq)^(2+)`

The oxidation number is balanced by adding one electron as:

`Mn_((aq))^(3+) + e^(-) -> Mn_(aq)^(2+)`  ....(ii)

The balanced chemical equation can be obtained by adding equation (i) and (ii) as:

`2Mn_(aq)^(3+) + 2H_2O_(l) -> MnO_(2(s)) + 2Mn_((aq))^(2+) + 4H_((aq))^(+)`

  Is there an error in this question or solution?
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APPEARS IN

NCERT Class 11 Chemistry Textbook
Chapter 8 Redox Reactions
Q 21 | Page 274
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