Enthalpy of neutralization of `CH_(3)COOH` by NaOH is less than that of HCl by NaOH.
Enthalpy of neutralization of `CH_(3)COOH` is less because of the absorption of heat in the ionization process.

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-15
B. If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-15
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the question regarding the enthalpy of neutralization of acetic acid (CH₃COOH) by sodium hydroxide (NaOH) compared to hydrochloric acid (HCl) by NaOH, we can break down the explanation into several steps:

### Step-by-Step Solution:

1. **Understanding Enthalpy of Neutralization**:
- The enthalpy of neutralization is the heat change that occurs when an acid reacts with a base to form water and a salt. It is usually expressed in kilojoules per mole of water formed.

2. **Neutralization of Strong Acid (HCl)**:
- When HCl (a strong acid) reacts with NaOH (a strong base), it dissociates completely into ions:
\[ \text{HCl} \rightarrow \text{H}^+ + \text{Cl}^- \]
\[ \text{NaOH} \rightarrow \text{Na}^+ + \text{OH}^- \]
- The reaction can be represented as:
\[ \text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O} \]
- The enthalpy change for this reaction is approximately -57 kJ/mol, indicating that a significant amount of heat is released.

3. **Neutralization of Weak Acid (CH₃COOH)**:
- Acetic acid (CH₃COOH) is a weak acid and does not dissociate completely in solution:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]
- The ionization of acetic acid requires energy, which is absorbed from the surroundings (endothermic process).

4. **Reaction with NaOH**:
- When acetic acid reacts with NaOH, the reaction can be represented as:
\[ \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \]
- The formation of water still releases energy, but since energy was absorbed during the ionization of acetic acid, the overall enthalpy change will be less than that of the strong acid.

5. **Conclusion**:
- Therefore, the enthalpy of neutralization of acetic acid by NaOH is less than that of HCl by NaOH due to the energy absorbed during the ionization of acetic acid. This explains why the enthalpy change for the neutralization of CH₃COOH is lower than that for HCl.

### Final Statement:
- The enthalpy of neutralization of CH₃COOH by NaOH is less than that of HCl by NaOH because the ionization of acetic acid absorbs heat, resulting in a lower overall enthalpy change.