How do you balance a reduction-oxidation or redox reaction?

Follow these 6 steps NOTE: This is NOT the same as balancing a regular chemical reaction! Please see the related question to the bottom of this answer for how to balance a normal chemical reaction. This is for oxidation-reduction, or redox reactions ONLY!

These instructions are for how to balance a reduction-oxidation, or redox reaction in aqueous solution, for both acidic and basic solution. Just follow these steps! I will illustrate each step with an example.

The example will the dissolution of copper(II) sulfide in aqueous nitric acid, shown as the following unbalanced reaction: CuS (s) NO 3 (aq) Cu 2 (aq) SO 4 2 (aq) NO (g) Step 1: Write two unbalanced half-reactions, one for the species that is being oxidized and its product, and one for the species that is reduced and its product Here is the unbalanced half-reaction involving CuS: CuS (s) Cu 2 (aq) SO 4 2 (aq) And the unbalanced half-reaction for NO 3 is.

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