Recap - Permanganate

Part of the Oxidation and Reduction section of Coddy's Chemistry journey. Lesson 15 of 27.

Challenge

The oxalate in spinach and rhubarb, C₂O₄²⁻, is measured with permanganate in acid. The purple color vanishes until all the oxalate is used up: MnO₄⁻ + H⁺ + C₂O₄²⁻ → Mn²⁺ + CO₂ + H₂O. Balance the equation.

Try it yourself

Equation balancerBalance the equation

MnO₄⁻H⁺C₂O₄²⁻Mn²⁺CO₂H₂O

All lessons in Oxidation and Reduction

1Electron Transfer

What Is Oxidation Oxidation Numbers Rules for Oxidation Numbers Oxidation Numbers in Ions Recap - Number Painter

4Metals and Reactivity

The Reactivity Series Displacement Reactions Metals and Acids Corrosion and Rust Recap - Metal Contest

2Redox Reactions

Spotting Redox Oxidizing Agents Reducing Agents Electrons Passed Recap - Who Gave Electrons

5Electrochemistry

Electrolysis Electrolysis of Melts Cells and Batteries Recap - Smelter

3Half-Equations

Writing Half-Equations Balancing with Electrons Half-Equations in Acid Combining Half-EquationsRecap - Permanganate

6Practice Problems

Recap - Bleach and Iodide Recap - Copper and Silver Recap - Bromine Redox