The correct order of increasing acidic strength is

(A) Ethanol
(B) Phenol
(C) Chloroacetic acid
(D) Acetic acid

Choose the correct answer from the options given below:

(A), (B), (D), (C)

The correct answer is Option (1) → (A), (B), (D), (C)

Acidic strength depends on stability of the conjugate base. Greater stability of conjugate base increases acidity. Electron withdrawing groups increase acidity, while resonance stabilization also enhances acidic strength.

Explanation

Option A: Ethanol Ethanol forms ethoxide ion after losing H⁺. This ion is not resonance stabilized and the negative charge remains localized on oxygen. Also, the alkyl group shows +I effect which destabilizes the conjugate base. Hence, ethanol is the weakest acid among the given.

Option B: Phenol Phenol forms phenoxide ion which is resonance stabilized. The negative charge is delocalized over the aromatic ring, making the conjugate base more stable than ethoxide. Thus, phenol is more acidic than ethanol.

Option D: Acetic acid Acetic acid forms acetate ion, where the negative charge is delocalized over two oxygen atoms by resonance. This provides greater stabilization than phenoxide ion. Therefore, acetic acid is more acidic than phenol.

Option C: Chloroacetic acid Chloroacetic acid contains an electron withdrawing chlorine atom which stabilizes the conjugate base via −I effect. This increases acidity significantly compared to acetic acid. Hence, it is the strongest acid among the given.

Increasing order of acidity Ethanol < Phenol < Acetic acid < Chloroacetic acid