NCERT Solution
Class 11
Chemistry
Redox Reactions
the mn3 ion is unstable in solution and undergoes...

Question:
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.

Answer:

The given reaction can be represented as:

Mn3+(aq) → Mn2+(aq) + MnO2(s) + H+(aq)

The oxidation half equation is:

M+3 n3+(aq) → M+4 nO2(s)

The oxidation number is balanced by adding one electron as:

Mn³⁺_(aq) → M nO_2(s) + e^-

The charge is balanced by adding 4H⁺ ions as:

Mn³⁺_(aq) → M nO_2(s) + 4H⁺_(aq) + e^-

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

Mn³⁺_(aq) + 2H2O(l) → MnO_2(s) + 4H⁺_(aq) + e^-..... (i)

The reduction half equation is:

Mn³⁺_(aq) → Mn²⁺_(aq)

The oxidation number is balanced by adding one electron as:

Mn³⁺_(aq) + e^- → Mn²⁺_(aq) ....... (ii)

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

2Mn³⁺_(aq) + 2H₂O_(l) → MnO_2(s) + 2Mn²⁺_(aq) + 4H⁺_(aq)

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Question:
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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Question: 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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Question:
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.