Question

would so₄²⁻ be used as an oxidizing agent or reducing agent in the reaction: so₄²⁻→s²⁻ reducing agent oxidizing agent

Explanation:

Step1: Calculate oxidation states

In \(SO_{4}^{2 -}\), let oxidation state of \(S\) be \(x\). Using formula \(x+4\times(- 2)=-2\) (since oxidation state of \(O\) is \(-2\)), we get \(x = +6\). In \(S^{2 -}\), oxidation state of \(S\) is \(-2\).

Step2: Determine agent type

Oxidation state of \(S\) changes from \(+6\) to \(-2\) (reduction). A species that undergoes reduction acts as an oxidizing agent.

Answer:

oxidizing agent