When potassium permanganate is added to acidulated solution of ferrous sulphate-

Options

A. Potassium ion is reduced
B. Manganese ions is oxidised
C. Ferrous ion is oxidised
D. Acid is neutralised

Answer

To solve the question regarding the reaction between potassium permanganate (KMnO4) and an acidulated solution of ferrous sulfate (FeSO4), we will follow these steps:

### Step 1: Identify the Reactants
We are given potassium permanganate (KMnO4) and ferrous sulfate (FeSO4) in an acidulated solution, which typically means sulfuric acid (H2SO4) is present.

### Step 2: Write the Reaction
The balanced chemical reaction between KMnO4 and FeSO4 in an acidic medium can be represented as follows:

\[ \text{KMnO}_4 + \text{FeSO}_4 + \text{H}_2\text{SO}_4 \rightarrow \text{MnSO}_4 + \text{K}_2\text{SO}_4 + \text{Fe}_2(\text{SO}_4)_3 + \text{H}_2\text{O} \]

### Step 3: Balance the Reaction
To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides. The balanced equation is:

\[ 2 \text{KMnO}_4 + 5 \text{FeSO}_4 + 8 \text{H}_2\text{SO}_4 \rightarrow 2 \text{MnSO}_4 + K_2\text{SO}_4 + 5 \text{Fe}_2(\text{SO}_4)_3 + 8 \text{H}_2\text{O} \]

### Step 4: Determine Oxidation States
- **Manganese (Mn)** in KMnO4 is in the +7 oxidation state.
- **Iron (Fe)** in FeSO4 is in the +2 oxidation state.
- After the reaction, Mn is reduced to +2 in MnSO4, and Fe is oxidized to +3 in Fe2(SO4)3.

### Step 5: Identify Changes in Oxidation States
- Manganese changes from +7 to +2 (reduction).
- Iron changes from +2 to +3 (oxidation).

### Step 6: Conclusion on Oxidation and Reduction
- Potassium (K) remains in the +1 oxidation state throughout the reaction, so it is neither oxidized nor reduced.
- The ferrous ion (Fe²⁺) is oxidized to ferric ion (Fe³⁺).
- The manganese ion (Mn) is reduced from +7 to +2.

### Final Answer
In this reaction, the ferrous ion (Fe²⁺) is oxidized to ferric ion (Fe³⁺), while manganese (Mn) is reduced from +7 to +2.