Q.Which one of the following is the Strongest acid ?

Showing the 12 most recent of 30 on this concept.

1. CBSE 2026Set V11 markMCQ
   Q.Given below are two statements : Statement I : Alcohols are acidic in nature; The acidic character of alcohol is due to the polar nature of the O–H bond in it. Statement II : Alcohols are weaker acids than water. In the light of the above statements, choose the most appropriate answer from the options given below :

   (a) Statement I is incorrect but Statement II is correct

   (b) Both Statement I and Statement II are correct

   (c) Both Statement I and Statement II are incorrect

   (d) Statement I is correct but Statement II is incorrect

   ›Reveal solutionSolution

   Alcohols are weakly acidic because of the polar O–H bond, and they are weaker acids than water — both statements are correct, so option (b).

   Statement I (correct): Alcohols show weak acidic character because the O–H bond is polar; the more electronegative oxygen pulls electron density from hydrogen, so it can be released as a proton:

   $\text{R–O–H} \rightleftharpoons \text{R–O}^- + \text{H}^+$ …

   🔒 Start your 14-day free trial to see the full solution →
2. CBSE 2026Set ANNUAL1 markMCQ
   Q.p-nitrophenol is stronger acid than phenol because nitro group is:

   (a) Electron donating

   (b) Electron withdrawing

   (c) Acidic

   (d) Basic

   ›Reveal solutionSolution

   p-Nitrophenol is more acidic than phenol because the -NO2 group is electron-withdrawing, stabilising the conjugate-base phenoxide ion.

   The acidity of phenols depends on how readily they lose the phenolic proton and how stable the resulting phenoxide (conjugate base) anion is. Substituents that WITHDRAW electron density (by −I inductive effect and/or −M resonance effect) delocalise and stabilise the negative charge on the phenoxide ion, increasing acidity. Substituents that DONATE electron density destabilise the negative charge (concentrate it), decreasing acidity.

   …

   🔒 Start your 14-day free trial to see the full solution →
3. CBSE 2026Set ANNUAL1 markMCQ
   Q.Phenol is more acidic than ethanol because

   (a) ethoxide ion is more stable than phenoxide ion

   (b) phenoxide ion is more stable than ethoxide ion

   (c) phenol undergoes electrophilic substitution reaction

   (d) phenol undergoes protonation easily

   ›Reveal solutionSolution

   Acid strength tracks conjugate-base stability; the phenoxide ion is resonance-stabilised by the aromatic ring while the ethoxide ion is not, so phenol is the stronger acid.

   Phenoxide ion, $C_6H_5O^-$: the negative charge on oxygen can delocalise into the ring through resonance, placing partial negative charge at the ortho and para carbons as well — several resonance structures share and spread out the charge, lowering the ion's energy (stabilising it).

   Ethoxide ion, $CH_3CH_2O^-$: there is no adjacent $\pi$ system to delocalise into, so the negative charge stays fully localised on the single oxygen atom; the electron-donating (+I) ethyl group actually intensifies (destabilises) this concentrated negative charge further.

   …

   🔒 Start your 14-day free trial to see the full solution →
4. CBSE 2026Set ANNUAL1 markMCQ
   Q.When Phenol is distilled with zinc powder, it gives-

   (a)

   (i) Benzene

   (b)

   (ii) Toluene

   (c)

   (iii) Benzaldehyde

   (d)

   (iv) Benzoic acid

   ›Reveal solutionSolution

   On distillation with zinc dust, phenol is reduced (the –OH group is removed) to give benzene. Correct option: (i).

   Concept. Zinc dust is a reducing agent that removes the hydroxyl group of phenol as zinc oxide, replacing the C–OH bond with a C–H bond.

   Reaction.

   $\text{C}_6\text{H}_5\text{OH} + \text{Zn} \xrightarrow{\Delta} \text{C}_6\text{H}_6 + \text{ZnO}$

   …

   🔒 Start your 14-day free trial to see the full solution →
5. CBSE 2026Set SEM31 markMCQ
   Q.The order of acidic strength for the following compounds is: (I) phenol (C6H5OH), (II) 4-nitrophenol, (III) 4-methylphenol, (IV) 2-nitrophenol

   (a) II > I > III > IV

   (b) II > IV > I > III

   (c) IV > II > I > III

   (d) IV > II > III > I

   ›Reveal solutionSolution

   Electron-withdrawing -NO2 raises phenol acidity, electron-donating -CH3 lowers it: 4-nitrophenol > 2-nitrophenol > phenol > 4-methylphenol. Correct option (b).

   Acidity of phenols depends on stabilisation of the phenoxide ion:

   • (II) 4-nitrophenol: -NO2 at para withdraws electrons by -I and -R, strongly stabilising the phenoxide -> most acidic (pKa ~ 7.1).
   • (IV) 2-nitrophenol: -NO2 at ortho is also strongly acidifying (pKa ~ 7.2); it is slightly less acidic than the para isomer largely due to intramolecular hydrogen bonding effects, but still far more acidic than phenol.
   • (I) phenol: reference (pKa ~ 10.0). …

   🔒 Start your 14-day free trial to see the full solution →
6. CBSE 2025Set ANNUAL1 markMCQ
   Q.The correct order of increasing acidic strength is:

   (a) Phenol < Ethanol < Chloroacetic acid < Acetic acid.

   (b) Ethanol < Phenol < Chloroacetic acid < Acetic acid.

   (c) Ethanol < Phenol < Acetic acid < Chloroacetic acid.

   (d) Chloroacetic acid < Acetic acid < Phenol < Ethanol.

   ›Reveal solutionSolution

   Acidic strength increases in the order Ethanol (weakest) < Phenol < Acetic acid < Chloroacetic acid (strongest), based on how well each conjugate base stabilizes the negative charge.

   • Ethanol ($pK_a \approx 16$): the ethoxide ion ($C_2H_5O^-$) has no way to delocalize its negative charge — it is the weakest acid of the four.
   • Phenol ($pK_a \approx 10$): the phenoxide ion is resonance-stabilized by delocalization of the negative charge into the benzene ring, making phenol far more acidic than ethanol, though still weaker than carboxylic acids.
   • Acetic acid ($pK_a \approx 4.76$): the acetate ion is stabilized by resonance between the two equivalent C–O bonds (much stronger stabilization than phenoxide's ring delocalization), making carboxylic acids much stronger acids than phenols. …

   🔒 Start your 14-day free trial to see the full solution →
7. CBSE 2025Set ANNUAL1 markMCQ
   Q.Assertion (A): Phenol is more acidic than ethanol. Reason (R): The phenoxide ion formed after loss of proton from phenol is stabilized by resonance, whereas the ethoxide ion is not.

   (a) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).

   (b) Both Assertion (A) and Reason (R) are true but Reason (R) is not correct explanation of Assertion (A).

   (c) Assertion (A) is true but Reason (R) is false.

   (d) Assertion (A) is false but Reason (R) is true.

   ›Reveal solutionSolution

   Phenol is indeed more acidic than ethanol, and the reason given — resonance stabilization of the phenoxide ion versus no such stabilization for the ethoxide ion — is exactly the correct explanation.

   Assertion: Phenol ($pK_a \approx 10$) is more acidic than ethanol ($pK_a \approx 16$). This is a well-established fact — TRUE.

   Reason: When phenol loses its $-OH$ proton, the resulting phenoxide ion ($C_6H_5O^-$) has its negative charge delocalized into the aromatic ring through resonance (the O⁻ lone pair conjugates with the ring's π system), spreading the charge over several ring carbons and stabilizing the ion. In contrast, the ethoxide ion ($C_2H_5O^-$) formed from ethanol has no adjacent π system to delocalize into — the negative charge stays local …

   🔒 Start your 14-day free trial to see the full solution →
8. CBSE 2025Set ANNUAL1 markMCQ
   Q.Which one of the following is the Strongest acid ?

   (a) 4-nitrophenol

   (b) 2-nitrophenol

   (c) 3-nitrophenol

   (d) 4-chlorophenol

   ›Reveal solutionSolution

   A $-NO_2$ group at the para position withdraws electron density from the phenolic $-OH$ by both resonance and induction, and (unlike the ortho isomer) without any competing intramolecular hydrogen bonding to the un-ionised $-OH$ — so 4-nitrophenol stabilises its conjugate-base phenoxide ion the most and is the strongest acid of the four options.

   Why nitrophenols are more acidic than phenol: the electron-withdrawing $-NO_2$ group pulls electron density away from the $-OH$ oxygen (destabilising the neutral acid, weakening the $O-H$ bond) and, once the proton is lost, delocalises the resulting negative charge of the phenoxide ion onto its own oxygen atoms by resonance — strongly stabilising the conjugate base and shifting the ionisation equilibrium further towards dissociation. Both effects make nitrophenols far more acidic than phenol itself.

   …

   🔒 Start your 14-day free trial to see the full solution →
9. CBSE 2024Set B1 mark
   Q.Write True or False: Phenols is also called carbolic acids.

   ›Reveal solutionSolution

   Phenol (C6H5OH) is indeed also called carbolic acid, historically used as an antiseptic.

   Phenol was one of the earliest antiseptics used in surgery (by Joseph Lister), and its common/trade name from that era, 'carbolic acid', is still widely used alongside the systematic name phenol. Its wea …

   🔒 Start your 14-day free trial to see the full solution →
10. CBSE 2024Set ANNUAL1 markMCQ
    Q.Mark the correct order of decreasing acid strength of the following compounds:

    (a) phenol (OH on benzene ring)

    (b) p-nitrophenol (OH with NO2 group para to it on the ring)

    (c) p-methoxyphenol (OH with OCH3 group para to it on the ring)

    (a) b > a > c

    (b) a > b > c

    (c) c > a > b

    (d) c > b > a

    ›Reveal solutionSolution

    Acidity of a substituted phenol depends on how well the ring substituent stabilises the resulting phenoxide anion: electron-withdrawing groups (like -NO2) increase acid strength, electron-donating groups (like -OCH3) decrease it.

    1. Phenol - the reference compound (moderate acidity, phenoxide stabilised only by ring delocalisation).
    2. p-nitrophenol - the -NO2 group is strongly electron-withdrawing (by both resonance and induction) at the para position, which further delocalises and stabilises the negative charge on the phenoxide oxygen, making the O-H bond easier to break -> MORE acidic than phenol. …

    🔒 Start your 14-day free trial to see the full solution →
11. CBSE 2024Set ANNUAL1 markMCQ
    Q.Which of the following is most acidic ?

    (a) Benzyl alcohol

    (b) Cyclohexanol

    (c) Phenol

    (d) m-Chlorophenol

    ›Reveal solutionSolution

    Phenols are more acidic than simple alcohols because the phenoxide ion is resonance-stabilised; an electron-withdrawing substituent like –Cl further stabilises the phenoxide and increases acidity beyond phenol itself.

    Acidity here depends on how well the conjugate base (the anion left after losing $H^+$) is stabilised:

    • Benzyl alcohol and cyclohexanol are simple alcohols; their alkoxide ions have no resonance stabilisation, so they are the weakest acids of the four (cyclohexanol is even weaker than benzyl alcohol since the benzylic system gives benzyl alcohol slight extra stabilisation, but both are far less acidic than any phenol).
    • Phenol is more acidic than alcohols because the phenoxide ion delocalises its negative charge into the aromatic ring via resonance. …

    🔒 Start your 14-day free trial to see the full solution →
12. CBSE 2024Set ANNUAL1 mark
    Q.Write the ascending order of acidic strength of the following compound. (I) Phenol (II) Meta nitro phenol (III) p-Nitro phenol

    ›Reveal solutionSolution

    The -NO2 group withdraws electron density and stabilises the phenoxide ion; this stabilisation is strongest when -NO2 is para (direct resonance) and weaker, but still present, when meta (only inductive).

    Acidic strength of a substituted phenol depends on how well the conjugate base (phenoxide ion, C6H5O-) is stabilised.

    • Phenol (I): No substituent; the phenoxide ion is stabilised only by resonance delocalisation over the ring — weakest acid of the three (pKa ~ 10.0).
    • m-Nitrophenol (II): The -NO2 group at the meta position cannot conjugate directly with the O- (no resonance structure places the negative charge on the carbon bearing NO2), so it stabilises the phenoxide ion only through its electron-withdrawing inductive effect. This makes it more acidic than plain phenol, but less acidic than the para isomer (pKa ~ 8.3). …

    🔒 Start your 14-day free trial to see the full solution →