The rate constant for the hydrolyiss of ethyl acetate in the presence of `0.1 N` acid `(A)` was found to be `5.4 xx 10^(5) s^(-1)` and for the hydrolyiss of ethyl acetate in the presence of `0.1 N` acid `(B)` , it was `6.2 xx 10^(-5) s^(-1)`. form these observations, one may conclude that

Options

A. A. Acids `(A)` and `(B)` are both of same strength.
B. B. Acid `(B)` is weaker than acid `(A)`.
C. C. Acid `(B)` is stronger than acid `(A)`.
D. D. Data in insufficient.

Answer

To solve the problem, we need to analyze the given rate constants for the hydrolysis of ethyl acetate in the presence of two different acids, A and B, both at the same concentration of 0.1 N.

### Step-by-Step Solution:

1. **Identify the Given Data**:
- Rate constant for hydrolysis with acid A, \( k_A = 5.4 \times 10^{-5} \, \text{s}^{-1} \)
- Rate constant for hydrolysis with acid B, \( k_B = 6.2 \times 10^{-5} \, \text{s}^{-1} \)

2. **Understand the Relationship Between Rate Constant and Acid Strength**:
- The rate of a reaction is directly proportional to the rate constant \( k \) when the concentration of reactants is constant.
- A higher rate constant indicates a faster reaction, which typically suggests that the acid is stronger.

3. **Compare the Rate Constants**:
- We compare \( k_A \) and \( k_B \):
- \( k_A = 5.4 \times 10^{-5} \)
- \( k_B = 6.2 \times 10^{-5} \)
- Since \( k_B > k_A \), this indicates that the reaction proceeds faster in the presence of acid B.

4. **Draw Conclusions About the Acids**:
- Since both acids are at the same concentration (0.1 N), the difference in rate constants implies that acid B is a stronger acid than acid A.
- A stronger acid will dissociate more completely in solution, leading to a higher concentration of hydrogen ions, which in turn increases the rate of the hydrolysis reaction.

5. **Final Conclusion**:
- Based on the comparison of the rate constants, we conclude that acid B is stronger than acid A.

### Conclusion:
- **Answer**: Acid B is stronger than acid A.

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