A: Enthalpy of neutralisation of 1 equivalent each of `HCI ` and `H_(2)SO_(4)` with NaOh is same.
R : Enthalpy of neutralisation is always the heat evolved when 1 mole acis is neutralised by a base.

Options

A. If both Assertion & Reason are true and the reason is the correct explanation of the assertion , then mark (1)
B. If both Assertion & Reason are true and the reason is not the correct explanation of the assertion, then mark (2)
C. If Assertion is true statement but Reason is false, then mark (3)
D. If both Assertion is true statement but Reason is false, then mark (3)

Answer

To solve the question regarding the enthalpy of neutralization of HCl and H₂SO₄ with NaOH, we will analyze the statements provided and derive conclusions based on the principles of thermodynamics.

### Step-by-Step Solution:

1. **Understanding Enthalpy of Neutralization:**
The enthalpy of neutralization is defined as the heat change that occurs when one equivalent of an acid reacts with one equivalent of a base to form water and a salt.

2. **Neutralization of HCl with NaOH:**
When hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH), the reaction can be represented as:
\[ \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \]
For this reaction, one mole of HCl (which provides 1 mole of H⁺ ions) reacts with one mole of NaOH (which provides 1 mole of OH⁻ ions) to produce 1 mole of water. The enthalpy change for this reaction is approximately -57.1 kJ/mol.

3. **Neutralization of H₂SO₄ with NaOH:**
When sulfuric acid (H₂SO₄) reacts with sodium hydroxide, the reaction can be represented as:
\[ \text{H}_2\text{SO}_4 + 2\text{NaOH} \rightarrow \text{Na}_2\text{SO}_4 + 2\text{H}_2\text{O} \]
Here, one mole of H₂SO₄ can provide 2 moles of H⁺ ions. Therefore, to neutralize 1 equivalent of H₂SO₄, we need to use 2 moles of NaOH. The enthalpy change for this reaction is also approximately -57.1 kJ for each mole of water formed.

4. **Equivalence in Reactions:**
When we consider one equivalent of H₂SO₄, we are actually considering half a mole of H₂SO₄ (since it can provide 2 H⁺ ions). Thus, when we react this half mole with 1 mole of NaOH, we still produce 1 mole of water and the enthalpy change remains -57.1 kJ.

5. **Conclusion:**
Both reactions, when considered in terms of equivalents, yield the same enthalpy of neutralization. Therefore, the statement A is true: the enthalpy of neutralization of 1 equivalent of HCl and H₂SO₄ with NaOH is the same.

6. **Evaluating Statement R:**
The statement R claims that the enthalpy of neutralization is always the heat evolved when 1 mole of acid is neutralized by a base. This is misleading because the enthalpy of neutralization is defined per equivalent, not per mole. The enthalpy change can vary with different acids and bases when considering full moles instead of equivalents. Therefore, statement R is false.

### Final Answer:
- Statement A is true.
- Statement R is false.