Out of 2-chloroethanol and ethanol, which is more acidic and why?

NCERT Exemplar · Q23

Q. Out of 2-chloroethanol and ethanol, which is more acidic and why?

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Concept understanding — Acidity Of Phenol

Inductive Effect on Acidity – From Intuition to Precision

Imagine you are holding a rope tied to a heavy box. If you pull the rope, the box moves toward you. Now imagine the rope is made of rubber bands — the pull still reaches the box, but it gets weaker the farther away you are. That is exactly how the inductive effect works inside a molecule.

The Core Intuition

An acid donates a proton ( $H^+$ ). After it does, the remaining part (the conjugate base) carries a negative charge. The stability of that negative charge determines how willing the molecule is to give up the proton. More stable conjugate base → stronger acid.

Now, some atoms or groups are electron-withdrawing — they pull electron density toward themselves through the sigma bonds. If such a group is attached near the acidic proton, it pulls some electron density away from the negative charge on the conjugate base. That spreads out (delocalises) the negative charge, making the conjugate base more stable. The acid becomes stronger.

Conversely, electron-donating groups push electron density toward the negative charge, concentrating it and making the conjugate base less stable. The acid becomes weaker.

Note

The inductive effect operates through sigma bonds only. It does not involve pi bonds or resonance. It is a permanent, through-bond polarisation.

The Precise Statement

Inductive effect on acidity: The acidity of a compound increases with the presence of electron-withdrawing groups (EWGs) near the acidic site, and decreases with electron-donating groups (EDGs). The effect is strongest when the group is closest to the acidic proton, and diminishes rapidly with distance.

Mathematically, for a series of substituted carboxylic acids:

\text{R-COOH} \quad \text{where R = substituent}

The acid dissociation constant $K_a$ changes as:

If R is electron-withdrawing (e.g., $-\text{Cl}$ , $-\text{NO}_2$ , $-\text{CF}_3$ ): $K_a$ increases → stronger acid.
If R is electron-donating (e.g., $-\text{CH}_3$ , $-\text{C}_2\text{H}_5$ ): $K_a$ decreases → weaker acid.

Why Distance Matters

The inductive effect falls off with distance because sigma bonds are localised. Each bond attenuates the effect by roughly a factor of 2–3. For example, compare:

Compound	$pK_a$	Explanation
$\text{CH}_3\text{COOH}$	4.76	Reference (no EWG)
$\text{ClCH}_2\text{COOH}$	2.86	Cl withdraws through one bond
$\text{Cl}_2\text{CHCOOH}$	1.29	Two Cl atoms, stronger withdrawal
$\text{Cl}_3\text{CCOOH}$	0.65	Three Cl atoms, strongest withdrawal
$\text{CH}_3\text{CH}_2\text{COOH}$	4.87	Ethyl group is electron-donating (slightly weaker acid)

Notice: $\text{ClCH}_2\text{COOH}$ is about 100 times stronger than acetic acid ( $\Delta pK_a \approx 1.9$ ). But if the Cl is moved further away:

Compound	$pK_a$
$\text{ClCH}_2\text{CH}_2\text{COOH}$	4.08
$\text{ClCH}_2\text{CH}_2\text{CH}_2\text{COOH}$	4.52

The effect fades as the chlorine moves farther from the carboxyl group. …

Why this formula?

Acidity of Phenol: Why It's More Acidic Than Alcohols

Let's build this from first principles — understanding why phenol is acidic is the key to mastering organic chemistry.

1. The Core Observation

Phenol ( $\ce{C6H5OH}$ ) has a pKa ≈ 10, while ethanol ( $\ce{CH3CH2OH}$ ) has a pKa ≈ 16.

This means phenol is about 1 million times more acidic than a typical alcohol.

The question: Why does the O–H bond in phenol break so much more easily?

2. The Key: Stability of the Conjugate Base

Acidity is determined by the stability of the conjugate base after losing $\ce{H+}$ .

Alcohol conjugate base: $\ce{CH3CH2O-}$ (alkoxide ion) — negative charge is localized on oxygen.
Phenol conjugate base: $\ce{C6H5O-}$ (phenoxide ion) — negative charge is delocalized into the benzene ring.

The Resonance Explanation

The phenoxide ion has multiple resonance structures:

\ce{C6H5O-} \leftrightarrow \text{(several resonance forms where negative charge moves to ortho/para carbons)}

Draw the structures mentally:

One structure has the negative charge on oxygen.
Other structures show the negative charge on carbon atoms at the ortho and para positions of the ring.

This delocalization spreads the negative charge over more atoms, making the ion more stable.

Key principle: The more stable the conjugate base, the stronger the acid.

3. Why Alcohols Can't Do This

In an alkoxide ion ( $\ce{RO-}$ ), the negative charge is stuck on oxygen.

There are no empty p-orbitals or conjugated $\pi$ systems nearby to accept the charge.

Result: The alkoxide is less stable, so the alcohol is less acidic.

4. The Inductive Effect Also Helps (But Resonance Dominates)

The benzene ring is slightly electron-withdrawing (due to its $sp^2$ carbons being more electronegative than $sp^3$ ).

This inductive effect pulls electron density away from the O–H bond, making the proton slightly more positive and easier to remove.

However, resonance stabilization of the conjugate base is the dominant factor — inductive effects alone cannot explain the million-fold difference.

5. The Quantitative Picture (pKa Values)

Compound	pKa	Conjugate base stability
Ethanol	~16	Localized charge on O
Phenol	~10	Delocalized charge via resonance
Acetic acid	~4.76	Even more resonance (two O atoms)

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The acidity of alcohols is governed by the stability of the conjugate base (alkoxide ion). Electron-withdrawing groups (like chlorine) stabilise the alkoxide by inductive effect, making the alcohol more acidic. 2-Chloroethanol is more acidic than ethanol because the -Cl group pulls electron density away from the O⁻, stabilising the conjugate base.

Why This Works: Inductive Effects and Alcohol Acidity

The question is about alcohols, not phenol, but the underlying principle is the same one used for phenols: acidity depends on how easily the O–H bond breaks and how stable the resulting negative charge on oxygen is. For any compound with an –OH group, the more stable the conjugate base (the alkoxide ion, RO⁻), the stronger the acid.

In ethanol ( $\mathrm{CH_3CH_2OH}$ ), the ethyl group is electron-donating (through hyperconjugation and inductive effect). That destabilises the negative charge on the oxygen in $\mathrm{CH_3CH_2O^-}$ — it pushes electron density toward an already negative centre. Bad for acidity.

In 2-chloroethanol ( $\mathrm{ClCH_2CH_2OH}$ ), the chlorine atom is strongly electron-withdrawing (inductive effect). It pulls electron density through the sigma bonds, away from the O⁻. That stabilises the negative charge, making the conjugate base more stable and the alcohol more acidic.

Watch out

Do not confuse this with the resonance effect in phenol. Here, chlorine’s effect is purely inductive — it acts through sigma bonds, not pi bonds. There is no resonance stabilisation of the alkoxide in 2-chloroethanol.

Step-by-Step Reasoning

Identify the acidic site. Both compounds have an –OH group. The acidic proton is the one on oxygen. When it leaves, we get an alkoxide ion: $\mathrm{RO^-}$ .
Compare the substituents attached to the –OH carbon chain.
- Ethanol: $\mathrm{CH_3CH_2OH}$ → conjugate base: $\mathrm{CH_3CH_2O^-}$
- 2-Chloroethanol: $\mathrm{ClCH_2CH_2OH}$ → conjugate base: $\mathrm{ClCH_2CH_2O^-}$
Analyse the inductive effect of the substituent.
- In ethanol, the ethyl group ( $\mathrm{-CH_2CH_3}$ ) is weakly electron-donating (+I effect). It pushes electron density toward the oxygen, making the negative charge on O⁻ more concentrated and less stable. This raises the energy of the conjugate base, so ethanol is a weaker acid.
- In 2-chloroethanol, the chlorine atom is electron-withdrawing (−I effect). It pulls electron density away from the oxygen through the sigma bonds. This delocalises the negative charge over a larger volume, stabilising the alkoxide ion. The conjugate base is lower in energy, so the acid is stronger. …

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Common Mistakes: Acidity of 2-Chloroethanol vs Ethanol

✗ Mistake 1: Assuming Chlorine Always Increases Acidity

The error: Students think "chlorine is electron-withdrawing, so 2-chloroethanol must be more acidic."

Why it's wrong: The inductive effect of chlorine does increase acidity — but only if the negative charge on the conjugate base can be stabilised. In 2-chloroethanol, the chlorine is on the $\beta$ -carbon (two bonds away), so its inductive effect is weaker than if it were on the $\alpha$ -carbon.

Correct reasoning:

In ethanol ( $\text{CH}_3\text{CH}_2\text{OH}$ ), the conjugate base is ethoxide ( $\text{CH}_3\text{CH}_2\text{O}^-$ ).
In 2-chloroethanol ( $\text{ClCH}_2\text{CH}_2\text{OH}$ ), the conjugate base is $\text{ClCH}_2\text{CH}_2\text{O}^-$ .
The chlorine withdraws electron density through sigma bonds, but the effect diminishes with distance. The $\beta$ -position gives only a modest stabilisation of the alkoxide ion.

Result: 2-chloroethanol is more acidic than ethanol, but the difference is small — not dramatic.

✗ Mistake 2: Confusing Inductive Effect with Resonance

The error: Students treat the Cl–C bond as if it can stabilise the negative charge via resonance (like in phenol).

Why it's wrong:

Chlorine has lone pairs, but in an alkyl chloride, there is no conjugation with the $\text{O}^-$ centre. The negative charge is localised on oxygen.
Resonance stabilisation requires the lone pair on oxygen to be delocalised into an adjacent $\pi$ -system (e.g., aromatic ring in phenol).
In 2-chloroethanol, the $\text{O}^-$ is separated from Cl by two $\text{sp}^3$ carbons — no $\pi$ overlap possible.

Correct reasoning: Only the inductive effect operates here — no resonance.

✗ Mistake 3: Forgetting the Solvent/Medium Context

The error: Students compare gas-phase acidities without considering that in aqueous solution, solvation effects dominate.

Why it's wrong:

In water, the alkoxide ion is stabilised by hydrogen bonding.
The small inductive effect of chlorine is often masked by solvation differences.
In fact, ethanol and 2-chloroethanol have nearly identical pKa values in water (~15.9 vs ~15.5). The difference is only ~0.4 pKa units.

Correct reasoning: The question likely expects you to say 2-chloroethanol is slightly more acidic due to the inductive effect, but acknowledge that the difference is small. …

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Same / Similar Concept — real previous-year questions on the same or a closely similar concept, not this exact question.

Showing the 12 most recent of 30 on this concept.

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:

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

…

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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.

…

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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.

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

…

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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). …
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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. …
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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 …

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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.

…

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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 …

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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.

Phenol - the reference compound (moderate acidity, phenoxide stabilised only by ring delocalisation).

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. …
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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. …
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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). …
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Q.Out of 2-chloroethanol and ethanol, which is more acidic and why?

Concept understanding — Acidity Of Phenol

Inductive Effect on Acidity – From Intuition to Precision

The Core Intuition

The Precise Statement

Why Distance Matters

Why this formula?

Acidity of Phenol: Why It's More Acidic Than Alcohols

1. The Core Observation

2. The Key: Stability of the Conjugate Base

The Resonance Explanation

3. Why Alcohols Can't Do This

4. The Inductive Effect Also Helps (But Resonance Dominates)

5. The Quantitative Picture (pKa Values)

Why This Works: Inductive Effects and Alcohol Acidity

Step-by-Step Reasoning

Method: Inductive Effect Analysis for Acidity Comparison

Step 1: Recall the acidity principle for alcohols

Step 2: Draw the conjugate bases

Step 3: Compare the inductive effects on the alkoxide ion

Step 4: Apply the stability–acidity relationship

Common Mistakes: Acidity of 2-Chloroethanol vs Ethanol

✗ Mistake 1: Assuming Chlorine Always Increases Acidity

✗ Mistake 2: Confusing Inductive Effect with Resonance

✗ Mistake 3: Forgetting the Solvent/Medium Context

Q.Out of 2-chloroethanol and ethanol, which is more acidic and why?

Why This Works: Inductive Effects and Alcohol Acidity

Step-by-Step Reasoning

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