Permanganate Reduction in Basic Solution

2MnO4− + H2O + 3e− → 2MnO2 + 4OH−

Overview

In basic or neutral solution, permanganate is reduced to manganese dioxide (MnO₂) rather than Mn²⁺. The purple solution produces a brown precipitate of MnO₂. This half-reaction is important in organic chemistry where KMnO₄ selectively oxidizes alkenes to diols under mild basic conditions (Baeyer test).

Participants

Role Substance Coefficient State
Reactant Water H₂O 1 (l)

Everyday Example

The Baeyer test uses cold dilute KMnO₄ to detect C=C double bonds in organic molecules, turning purple to brown with a precipitate.

Industrial Importance

Basic permanganate oxidation is used in organic synthesis for controlled oxidation of alkenes and in water treatment for taste and odor removal.

Properties

Type
Redox
Reversible
No
Energy
Exothermic

Related Reactions

Aqua Regia Dissolving Gold Bleaching with Sodium Hypochlorite Cerium(IV) Reduction by Iron(II) Chlorine Oxidation of Bromide Chromate-Dichromate Equilibrium Contact Process SO₂ Oxidation Copper Displaced by Iron Copper Oxidation by Nitric Acid Copper Patina Formation (Verdigris) Copper Reduction of Silver Ion

Frequently Asked Questions

What is the equation for Permanganate Reduction in Basic Solution?
The balanced equation is: 2MnO₄⁻ + H₂O + 3e⁻ → 2MnO₂ + 4OH⁻.
What type of reaction is Permanganate Reduction in Basic Solution?
Permanganate Reduction in Basic Solution is a redox reaction.
Is Permanganate Reduction in Basic Solution exothermic or endothermic?
Permanganate Reduction in Basic Solution is exothermic (releases energy).