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).