One of the products formed from the reaction of permanganate ion with iodide ion in neutral aqueous medium is:
Show Hint
- \( \text{I}_2 \)
- \( \text{IO}_3^- \)
- \( \text{IO}_4^- \)
\( \text{IO}_2^- \)
The Correct Option is B
Solution and Explanation
Step 1: Identify the oxidizing and reducing agents
In this redox reaction: - \( \text{MnO}_4^- \) (permanganate ion) acts as the \textit{oxidizing agent} (it gets reduced). - \( \text{I}^- \) (iodide ion) acts as the \textit{reducing agent} (it gets oxidized).
Step 2: Understand the medium and expected products
The products of redox reactions involving permanganate ion depend on the reaction medium: - In acidic medium: \( \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \) - In basic medium: \( \text{MnO}_4^- \rightarrow \text{MnO}_4^{2-} \) - In neutral medium: \( \text{MnO}_4^- \rightarrow \text{MnO}_2 \) So, since this is a neutral medium, permanganate will be reduced to \( \text{MnO}_2 \).
Step 3: Oxidation of iodide ion \( \text{I}^- \)
The iodide ion is oxidized to iodate ion \( \text{IO}_3^- \) in a neutral medium. This is a known redox behavior under these conditions.
Step 4: Balanced redox reaction
The balanced reaction is: \[ 2 \text{MnO}_4^- + \text{I}^- + \text{H}_2\text{O} \rightarrow 2 \text{MnO}_2 + \text{IO}_3^- + 2 \text{OH}^- \] This confirms that one of the products is \( \text{IO}_3^- \), the iodate ion.
Final Answer: \( \boxed{\text{IO}_3^-} \)
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