Question

Statement-I : \(\mathrm{KMnO_4}\) is a good reducing agent.
Statement-II : \(\mathrm{KMnO_4}\) reduces nitrite, oxalate and iodide ions.

• A. Both statements are correct.
• B. Both statements are incorrect.
• C. Statement I is correct while Statement II is incorrect.
• D. Statement I is incorrect while Statement II is correct.

Hint:

\(\mathrm{KMnO_4}\) almost always acts as an {oxidizing agent}. If a statement says it is reducing something, check carefully!

Answer 1

The Correct Option is B

To determine the correctness of the given statements about \mathrm{KMnO_4}, we need to analyze each statement individually and justify why the correct answer is that both statements are incorrect.

1. Statement I: \(\mathrm{KMnO_4}\) is a good reducing agent.
   • \(\mathrm{KMnO_4}\) is actually a strong oxidizing agent, not a reducing agent. It is commonly used in redox reactions where it oxidizes other compounds while itself getting reduced.
   • In acidic medium, manganese in \(\mathrm{KMnO_4}\) gets reduced from the +7 oxidation state to +2 oxidation state. Its function as an oxidizing agent makes the statement incorrect.
2. Statement II: \(\mathrm{KMnO_4}\) reduces nitrite, oxalate, and iodide ions.
   • As discussed, \(\mathrm{KMnO_4}\) serves as an oxidizing agent, not as a reducing one. Hence, it oxidizes nitrite, oxalate, and iodide ions rather than reducing them.
   • For example:
     • Oxidation of oxalate ions (\(\mathrm{C_2O_4^{2-}}\)) leads to \(\mathrm{CO_2}\), while \(\mathrm{KMnO_4}\) reduces to \(\mathrm{Mn^{2+}}\).
     • Iodide ions (\(\mathrm{I^-}\)) are oxidized to iodine (\(\mathrm{I_2}\)) by \(\mathrm{KMnO_4}\).
   • Hence, this statement is also incorrect as \(\mathrm{KMnO_4}\) does not reduce these ions.

After analyzing both statements, it is clear that both are incorrect because they mistakenly describe the properties and actions of \(\mathrm{KMnO_4}\) in redox reactions.

Conclusion: The correct answer is Both statements are incorrect.