Recap - Bleach and Iodide

Part of the Oxidation and Reduction section of Coddy's Chemistry journey. Lesson 25 of 27.

Challenge

Household bleach is a solution of sodium hypochlorite, NaClO. A quick test for it: a few drops added to colorless potassium iodide solution turn it brown, because iodine forms:

ClO⁻ + I⁻ + H₂O → Cl⁻ + I₂ + OH⁻

A colorless potassium iodide solution, and the same solution turned brown after a few drops of bleach

Bleach turns iodide into brown iodine

Name the element oxidized and the element reduced, choose the oxidizing agent and the reducing agent, and count the electrons passed in the balanced equation.

Try it yourself

Oxidation numbersFollow the electrons

ClO⁻I⁻H₂OCl⁻I₂OH⁻

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-Equations Recap - Permanganate

6Practice Problems

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