Q.Arrange the following in increasing order of their acidic character : Benzoic acid, Phenol, Cresol

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:

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

   Statement II (correct): Alcohols ($\text{p}K_a \approx 16\text{–}18$) are weaker acids than water ($\text{p}K_a \approx 15.7$). The alkyl group is electron-donating (+I effect), which increases electron density on oxygen, destabilises the alkoxide ion ($\text{RO}^-$) relative to hydroxide ($\text{OH}^-$), and so makes the alcohol a poorer proton donor than water.

   Both statements are therefore correct.

   ✓Final answer

   (b) Both Statement I and Statement II are correct

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.

   The nitro group ($-NO_2$) is a strong electron-withdrawing group, both inductively and by resonance (the nitrogen, being positively polarised, can accept electron density through the ring via conjugation, especially effective from the ortho/para positions). In p-nitrophenoxide, the negative charge on oxygen can be delocalised right onto the nitro group's oxygens through the conjugated ring, giving extra resonance stabilisation not available to plain phenoxide. This makes p-nitrophenol a noticeably stronger acid ($pK_a\approx7.2$) than phenol ($pK_a\approx10$).

   ✓Final answer

   (b) The nitro group is electron withdrawing, which stabilises the phenoxide ion and increases acid strength.

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.

   Because the phenoxide ion is markedly more stable than the ethoxide ion, the equilibrium $ArOH \rightleftharpoons ArO^- + H^+$ lies further to the right than $ROH \rightleftharpoons RO^- + H^+$, i.e. phenol ($pK_a \approx 10$) is a much stronger acid than ethanol ($pK_a\approx 16$).

   Why the other options are wrong: (a) is the reverse of the true stability order; (c) phenol's electrophilic-substitution behaviour on the ring is a separate property, unrelated to why it is acidic; (d) ease of protonation is irrelevant to acid strength, which is about the ease of losing a proton, not gaining one.

   ✓Final answer

   (b) phenoxide ion is more stable than ethoxide ion

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.

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

   This is a standard way to demonstrate that the phenolic –OH can be reductively removed. Toluene, benzaldehyde and benzoic acid would each require an extra carbon or an oxidation, which this reaction does not provide.

   ✓Final answer

   (i) Benzene — phenol distilled with zinc dust loses its –OH (as ZnO) to give benzene.

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).
   • (III) 4-methylphenol (p-cresol): -CH3 is electron donating (+I/hyperconjugation), destabilises the phenoxide -> least acidic (pKa ~ 10.3).

   Order: II > IV > I > III. Substituent effects on phenol acidity are a standard NCERT Class 12 Chemistry (Alcohols, Phenols and Ethers) topic.

   ✓Final answer

   (b) II > IV > I > III.

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.
   • Chloroacetic acid ($pK_a \approx 2.86$): the electronegative Cl atom exerts a $-I$ (inductive) effect that further withdraws electron density and stabilizes the carboxylate anion even more than in plain acetic acid, making it the strongest acid of the four.

   So the increasing order of acidic strength is: Ethanol < Phenol < Acetic acid < Chloroacetic acid.

   ✓Final answer

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

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 localized entirely on oxygen, making it much less stable — TRUE.

   Since a more stable (delocalized) conjugate base means an easier/more favourable loss of $H^+$, i.e., greater acidity, the Reason directly and correctly explains why phenol is more acidic than ethanol.

   ✓Final answer

   (a) Both A and R are true, and R correctly explains A.

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.

   Comparing positions of substitution: the $-NO_2$ group can donate its stabilising resonance effect to the ring's negative charge only from the ortho and para positions (not meta, where only the weaker inductive effect operates) — so 3-nitrophenol (meta), lacking resonance stabilisation, is the weakest acid of the three nitrophenol isomers. Between the ortho and para nitrophenols, the para isomer (4-nitrophenol) achieves fuller, unhindered resonance delocalisation of the phenoxide charge into the nitro group, whereas in 2-nitrophenol the adjacent $-OH$ and $-NO_2$ groups instead favour an intramolecular hydrogen bond in the un-ionised acid, which slightly stabilises the neutral (undissociated) form and modestly suppresses ionisation. The net effect is that 4-nitrophenol ($pK_a \approx 7.15$) is marginally more acidic than 2-nitrophenol ($pK_a\approx7.2$), and both are far more acidic than 3-nitrophenol ($pK_a\approx8.4$).

   4-chlorophenol is the weakest acid of the four options: chlorine is a much weaker electron-withdrawing group than $-NO_2$ (its resonance donation of electron density, a $+M$ effect from the lone pairs, partly offsets its $-I$ inductive withdrawal), so it stabilises the phenoxide ion far less ($pK_a\approx9.2$, only slightly more acidic than phenol's $\approx10.0$).

   ✓Final answer

   The correct answer is (a) 4-nitrophenol — the para-nitro group gives the strongest combined inductive + resonance stabilisation of the phenoxide ion, without the competing intramolecular H-bonding that slightly damps the acidity of the ortho isomer.

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 weakly acidic character (due to resonance stabilisation of the phenoxide ion) is consistent with this older name.

   ✓Final answer

   True.

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.
    3. p-methoxyphenol - the -OCH3 group is electron-DONATING by resonance, which pushes electron density towards the ring/oxygen and destabilises (concentrates) the negative charge on the phenoxide, making it harder to lose H+ -> LESS acidic than phenol. So decreasing acid strength: p-nitrophenol > phenol > p-methoxyphenol, i.e. b > a > c.

    ✓Final answer

    (a) b > a > c.

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.
    • m-Chlorophenol carries an electron-withdrawing chlorine (–I effect, dominant at the meta position since resonance donation from Cl into the ring cannot reach the ortho/para positions relative to Cl but still withdraws inductively) that further stabilises the phenoxide ion by dispersing negative charge, making it more acidic than phenol itself.

    Order of acidity: benzyl alcohol < cyclohexanol < phenol < m-chlorophenol.

    ✓Final answer

    (d) m-Chlorophenol.

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).
    • p-Nitrophenol (III): The -NO2 group at the para position CAN conjugate directly with the negative charge on oxygen through resonance (the negative charge can be delocalised onto the nitro-group oxygens), giving very strong stabilisation of the phenoxide ion — most acidic of the three (pKa ~ 7.15).

    So acidic strength increases: Phenol < m-nitrophenol < p-nitrophenol.

    ✓Final answer

    Ascending order of acidic strength: Phenol (I) < m-Nitrophenol (II) < p-Nitrophenol (III).