Question

One of the products formed from the reaction of permanganate ion with iodide ion in neutral aqueous medium is:

• A. \( \text{I}_2 \)
• B. \( \text{IO}_3^- \)
• C. \( \text{IO}_4^- \)
• D. \( \text{IO}_2^- \)

Hint:

In redox reactions involving permanganate ion, always consider the medium (acidic, basic, or neutral), as it determines the product formed by manganese. In neutral medium, \( \text{MnO}_4^- \) is reduced to \( \text{MnO}_2 \), and iodide typically oxidizes to \( \text{IO}_3^- \).

Answer 1

The Correct Option is B

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: \( \boxed{\text{IO}_3^-} \)