Statement-1: `H_(2)S` is weak diprotic acid.
Statement-2: Salt of aq. `Na_(2)S` has pH greater than 7.

Options

A. (a) Statement-1 is true, statement-2 is true, statement-2 is a correct explanation for statement-1
B. (b) Statement-1 is true, statement-2 is true, statement-2 is not correct explanation for statement-1
C. (c) Statement-1 is true, statement-2 is false
D. (d) Statement-1 is false, statement-2 is true

Answer

To solve the question, we need to evaluate the two statements provided:

**Statement 1:** H₂S is a weak diprotic acid.
**Statement 2:** Salt of aqueous Na₂S has pH greater than 7.

### Step 1: Analyze Statement 1
- **Definition of a Diprotic Acid:** A diprotic acid is one that can donate two protons (H⁺ ions).
- **Dissociation of H₂S:**
- In water, H₂S partially dissociates to form H⁺ and HS⁻ ions:
\[ \text{H}_2\text{S} \rightleftharpoons \text{H}^+ + \text{HS}^- \]
- The HS⁻ ion can further dissociate to release another H⁺ ion:
\[ \text{HS}^- \rightleftharpoons \text{H}^+ + \text{S}^{2-} \]
- **Conclusion:** Since H₂S does not completely dissociate and can donate two protons, it is classified as a weak diprotic acid. Therefore, **Statement 1 is true.**

### Step 2: Analyze Statement 2
- **Formation of Na₂S:** Sodium sulfide (Na₂S) is formed from the neutralization of a weak acid (H₂S) with a strong base (NaOH).
- **Nature of the Salt:**
- When a weak acid reacts with a strong base, the resulting salt is basic in nature.
- Na₂S will dissociate in water to give Na⁺ and S²⁻ ions. The S²⁻ ion can react with water to produce OH⁻ ions:
\[ \text{S}^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{HS}^- + \text{OH}^- \]
- **pH of Na₂S Solution:** The production of OH⁻ ions indicates that the solution will be basic, leading to a pH greater than 7. Therefore, **Statement 2 is true.**

### Step 3: Determine the Relationship Between the Statements
- **Statement 1 is true** because H₂S is indeed a weak diprotic acid.
- **Statement 2 is true** because the salt Na₂S has a pH greater than 7 due to its basic nature.
- **Explanation Relationship:** While both statements are true, Statement 2 does not explain Statement 1. The basicity of Na₂S does not provide a reason for H₂S being a weak diprotic acid.

### Conclusion
- Both statements are true, but Statement 2 is not a correct explanation for Statement 1. Therefore, the correct answer is **Option B**: Statement 1 is true, Statement 2 is true, and Statement 2 is not the correct explanation for Statement 1.

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