Question:medium
Assertion (A): Fluoroacetic acid is a stronger acid than chloroacetic acid.
Reason (R): This is due to greater electron-withdrawing nature of \( F \) than \( Cl \).
Assertion (A): Fluoroacetic acid is a stronger acid than chloroacetic acid.
Reason (R): This is due to greater electron-withdrawing nature of \( F \) than \( Cl \).
Show Hint
A stronger electron-withdrawing group increases acidity by stabilizing the conjugate base.
Updated On: Jan 13, 2026
- Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
- Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
- Assertion (A) is true, but Reason (R) is false
- Assertion (A) is false, but Reason (R) is true.
Show Solution
The Correct Option is A
Solution and Explanation
The greater electronegativity of fluorine compared to chlorine enhances the inductive (-I) effect in fluoroacetic acid. This stabilization of the carboxylate ion results in increased acidity relative to chloroacetic acid.
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