The correct option is
B o−nitrophenol
Analysing the factors affecting the acidic strengths of given compounds
- Electron withdrawing group increases the acidic strength and electron donating group decreases the acidic strength.
- Acidic strength ∝ stability of conjugate base
Analysing the options
Option (A):
Conjugate base of ethanol is ethoxide ion which is not stabilized by resonance:
Phenol is more acidic as compared to ethanol because conjugate base of phenol is stabilized by resonance:
Option (B):
Phenol will be less acidic as compared to
o−nitrophenol due to the presence of the electron withdrawing group
(−NO2) in
o−nitrophenol.
−NO2 group decreases electron density on oxygen atom of
−OH and makes release of
H+ easier.
Option (C):
o−methylphenol will be a little less acidic as compared to phenol because of the presence of electron donating group
(−CH3) at ortho position.
−CH3 group increases electron density on oxygen atom of
−OH and makes release of
H+ difficult.
Option (D):
o−methoxyphenol will be less acidic as compared to phenol because of the
+R effect of the methoxy group present at ortho position which makes the release of
H+ difficult.
So, the correct answer is option
(B).