Assertion : `H_(2)O_(2)` react with PbS to form `PbSO_(4)`.
Reason : `H_(2)O_(2)` is weak acid

Options

A. If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B. If both Assertion & Reason are True but Reason is not a correct explanation of the Assertion.
C. If Assertion is True but the Reason is False.
D. If both Assertion & Reason are False.

Answer

To solve the question, we need to analyze both the assertion and the reason provided.

### Step 1: Analyze the Assertion
The assertion states that hydrogen peroxide (H₂O₂) reacts with lead sulfide (PbS) to form lead sulfate (PbSO₄).

- **Chemical Reaction**: The reaction can be represented as:
\[ 4 \text{H}_2\text{O}_2 + \text{PbS} \rightarrow \text{PbSO}_4 + 4 \text{H}_2\text{O} \]
- **Balancing**: The reaction is balanced by ensuring that the number of atoms of each element is the same on both sides.

### Step 2: Analyze the Reason
The reason states that hydrogen peroxide (H₂O₂) is a weak acid.

- **Acidic Nature**: H₂O₂ can act as a weak acid due to the presence of hydrogen ions (H⁺) in its structure. However, its primary role in the reaction with PbS is not as an acid but as an oxidizing agent.

### Step 3: Determine the Role of H₂O₂
In the reaction:
- H₂O₂ acts as an oxidizing agent, converting PbS (where sulfur is in the -2 oxidation state) to PbSO₄ (where sulfur is in the +6 oxidation state).
- This indicates that H₂O₂ is undergoing reduction while PbS is being oxidized.

### Step 4: Conclusion
- **Assertion**: True, H₂O₂ does react with PbS to form PbSO₄.
- **Reason**: True, H₂O₂ is a weak acid, but this is not the reason for its reaction with PbS in this context.

### Final Answer
The assertion is correct, and the reason is also correct, but the reason does not correctly explain the assertion. Therefore, the answer is option B: "Assertion is correct, Reason is correct, but Reason is not the correct explanation of Assertion."

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