Question

What happens when \( \mathrm{H_2O_2} \) is added to an aqueous solution of ferrous sulphate in an acidic medium?

• A. Only $\mathrm{H_2O_2}$ is evolved
• B. $\mathrm{Fe}^{2+}$ is reduced
• C. $\mathrm{Fe}^{2+}$ is oxidized
• D. $\mathrm{H_2O_2}$ is evolved and $\mathrm{Fe}^{2+}$ is oxidized

Hint:

Understanding oxidation-reduction reactions is crucial for predicting chemical behavior in various environments.

Answer 1

The Correct Option is C

Analyze the redox behavior of \( \mathrm{H_2O_2} \) in reaction with \( \mathrm{Fe}^{2+} \).
\[ \mathrm{Fe}^{2+} + \mathrm{H_2O_2} \rightarrow \mathrm{Fe}^{3+} + \mathrm{H_2O} \]

This reaction primarily involves the oxidation of \( \mathrm{Fe}^{2+} \) to \( \mathrm{Fe}^{3+} \) by \( \mathrm{H_2O_2} \), which acts as an oxidizing agent.