The enthalpies of neutralization to two weak acids `HA` and `HB`
with `NaOH` are `-10.1` and `-11.8` `Kcal//g`. eq respectively.
Which of the following relation is correct regarding acidic
strengths of `HA` and `HB` `:-`

Options

A. `HAgtHB`
B. `HAltHB`
C. `HA=HB`
D. Cannot be predicted

Explanation

To determine the relationship between the acidic strengths of the weak acids \( HA \) and \( HB \) based on their enthalpies of neutralization with sodium hydroxide (\( NaOH \)), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Enthalpy of neutralization for \( HA \): \( \Delta H_{HA} = -10.1 \) Kcal/g eq
- Enthalpy of neutralization for \( HB \): \( \Delta H_{HB} = -11.8 \) Kcal/g eq

2. **Understand the Concept of Enthalpy of Neutralization:**
- The enthalpy of neutralization is the heat change when one gram equivalent of an acid is neutralized by a base (in this case, \( NaOH \)).
- A negative value indicates that the reaction is exothermic, meaning heat is released during the neutralization process.

3. **Analyze the Relationship Between Enthalpy of Neutralization and Acid Strength:**
- Generally, a stronger acid will have a more negative enthalpy of neutralization because it dissociates more completely in solution, releasing more heat during the neutralization.
- Conversely, a weaker acid will have a less negative (or higher) enthalpy of neutralization, indicating that it does not dissociate as completely.

4. **Compare the Enthalpy Values:**
- Since \( \Delta H_{HA} = -10.1 \) Kcal/g eq (less negative) and \( \Delta H_{HB} = -11.8 \) Kcal/g eq (more negative), we can conclude that:
- \( HB \) is a stronger acid than \( HA \) because it has a more negative enthalpy of neutralization.

5. **Establish the Conclusion:**
- Therefore, the correct relationship regarding the acidic strengths of \( HA \) and \( HB \) is:
\[ HB > HA \]

### Final Answer:
The correct relation regarding the acidic strengths of \( HA \) and \( HB \) is:
\[ HB > HA \]