Statement-1: HBr can be obtained by treating NaBr with `H_(3)PO_(4)`.
Statement-2: `H_(3)PO_(4)` is stronger acid than HBr.

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 both statements provided and determine their truthfulness.

### Step 1: Analyze Statement 1
**Statement 1**: HBr can be obtained by treating NaBr with H₃PO₄.

- **Explanation**: Sodium bromide (NaBr) reacts with phosphoric acid (H₃PO₄) to produce hydrogen bromide (HBr) and sodium phosphate (Na₃PO₄).
- **Chemical Reaction**:
\[ 3 \, \text{NaBr} + \text{H}_3\text{PO}_4 \rightarrow \text{Na}_3\text{PO}_4 + 3 \, \text{HBr} \]
- **Conclusion**: This reaction confirms that HBr can indeed be obtained from NaBr and H₃PO₄. Therefore, Statement 1 is **true**.

### Step 2: Analyze Statement 2
**Statement 2**: H₃PO₄ is a stronger acid than HBr.

- **Explanation**: To determine the strength of the acids, we can look at their dissociation constants (Ka).
- For H₃PO₄ (phosphoric acid), the dissociation constant (Ka) is approximately \(7.1 \times 10^{-3}\).
- For HBr (hydrogen bromide), the dissociation constant (Ka) is approximately \(1.0 \times 10^{9}\).
- **Comparison**: Since the Ka value for HBr is significantly higher than that of H₃PO₄, it indicates that HBr is a stronger acid than H₃PO₄.
- **Conclusion**: Therefore, Statement 2 is **false**.

### Step 3: Determine the Correct Option
- **Summary**:
- Statement 1 is true.
- Statement 2 is false.
- **Correct Option**: Based on the evaluations, the correct option is **C**: Statement 1 is true, Statement 2 is false.

### Final Answer
The correct answer is **C**: Statement 1 is true, Statement 2 is false.

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