Identify the correct products formed during the oxidizing reaction of permanganate ion with sulphite ion in acidic solution

A. \(2OH^-\)

B. \(2Mn^{2+}\)

C. \(3H_2O\)

D. \(MnO_2\)

E. \(5SO_4^{2-}\)

Choose the correct answer from the option given below:

B, C and E only

The correct answer is option 3. B, C and E only.

Let us break down the reaction and the products formed during the oxidizing reaction of permanganate ion (\(MnO_4^-\)) with sulfite ion (\(SO_3^{2-}\)) in acidic solution.

The balanced chemical equation for the reaction is:

\[ \text{2MnO}_4^- + \text{5SO}_3^{2-} + \text{6H}^+ \rightarrow \text{2Mn}^{2+} + \text{5SO}_4^{2-} + \text{3H}_2\text{O} \]

In this reaction:

Permanganate ion (\(MnO_4^-\)) acts as the oxidizing agent.

Sulphite ion (\(SO_3^{2-}\)) acts as the reducing agent.

The reaction takes place in acidic solution, so there are \(H^+\) ions present.

Here's what happens:

1. Permanganate ion oxidizes sulphite ion to sulfate ion.

\[ \text{MnO}_4^- + \text{SO}_3^{2-} \rightarrow \text{Mn}^{2+} + \text{SO}_4^{2-} \]

In this step, manganese in permanganate ion changes from \(+7\) oxidation state to \(+2\) oxidation state, while sulfur in sulfite ion changes from \(+4\) oxidation state to \(+6\) oxidation state.

2. Water molecules are formed as a result of the acidic medium.

\[ \text{H}_3\text{O}^+ + \text{SO}_3^{2-} \rightarrow \text{H}_2\text{O} + \text{HSO}_3^- \]

This step involves the acid-base reaction between hydronium ions (\(H_3O^+\)) and sulfite ions (\(SO_3^{2-}\)), leading to the formation of water (\(H_2O\)) and bisulfite ion (\(HSO_3^-\)).

So, the correct products formed during the reaction are:

\(2\) \(Mn^{2+}\)

\(3\) \(H_2O\)

\(5\) \(SO_4^{2-}\)

This matches with option 3: \(B\), \(C\), and \(E\) only.