Question

The reaction of H₂O₂ with potassium permanganate in acidic medium leads to the formation of mainly

• A. Mn²⁺
• B. Mn⁴⁺
• C. Mn³⁺
• D. Mn⁶⁺

Answer 1

The Correct Option is A

To understand the reaction between hydrogen peroxide (H₂O₂) and potassium permanganate (KMnO₄) in acidic medium, it is important to understand the redox behavior of permanganate ions (MnO₄^-) under acidic conditions.

The balanced chemical equation for the redox reaction of KMnO₄ with H₂O₂ in an acidic medium is as follows:

2KMnO_4 + 5H_2O_2 + 3H_2SO_4 \rightarrow 2MnSO_4 + K_2SO_4 + 8H_2O + 5O_2

In this reaction:

• Manganese in the permanganate ion (MnO₄^-) has an oxidation state of +7.
• The MnO₄^- ion gets reduced to Mn²⁺, as seen in the formation of MnSO₄.
• This transformation means a reduction by gaining electrons.

Since the oxidation state of manganese reduces from +7 in MnO₄^- to +2 in Mn²⁺, the main product formed in this acidic medium reaction is Mn²⁺.

Regarding the options:

• Mn²⁺: The correct answer, as it is the product formed in the acidic reduction of permanganate.
• Mn⁴⁺, Mn³⁺, and Mn⁶⁺: These are incorrect because they are not typically formed from permanganate oxidation in strongly acidic conditions.

Understanding redox reactions and recognizing the patterns of manganese's oxidation states in different media are crucial for solving such questions.