Practice MCQs for JEE Chemistry Equilibrium
Access targeted multiple-choice questions for Equilibrium designed to align with the latest JEE academic syllabus for JEE Chemistry. These objective practice sets help students evaluate their conceptual understanding and improve exam readiness.
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Multiple Choice Questions
(a) \( \ce{HF} \)
(b) \( \ce{HCl} \)
(c) \( \ce{HBr} \)
(d) \( \ce{HI} \)
Show Answer & Explanation
Answer: (a) \( \ce{HF} \)
Explanation:
1. Acid strength of hydrohalic acids increases down the group as the H-X bond becomes weaker; HF is the weakest.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) on increasing dilution
(b) on increasing pressure
(c) on decreasing dilution
(d) none of these
Show Answer & Explanation
Answer: (a) on increasing dilution
Explanation:
1. Dilution increases ionisation.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) 1
(b) 2
(c) 3
(d) 4
Show Answer & Explanation
Answer: (c) 3
Explanation:
1. \( \ce{H3PO4} \) is tribasic and loses its three protons in three successive steps.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) acidic
(b) neutral
(c) basic
(d) none of these
Show Answer & Explanation
Answer: (c) basic
Explanation:
1. \( \ce{HPO4^2-} \) hydrolyses (\( \ce{HPO4^2- + H2O <=> H2PO4- + OH-} \)) more than it ionises, so the solution is basic.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{HCl} \), NaOH
(b) \( \ce{NH4Cl} \), \( \ce{NH4OH} \)
(c) \( \ce{H2SO4} \), \( \ce{HSO4-} \)
(d) KCN, HCN
Show Answer & Explanation
Answer: (c) \( \ce{H2SO4} \), \( \ce{HSO4-} \)
Explanation:
1. The members of a pair differ by exactly one proton: \( \ce{H2SO4} \) minus \( \ce{H+} \) gives \( \ce{HSO4-} \).
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{H3PO4} \)
(b) \( \ce{H3PO3} \)
(c) \( \ce{H2PO3-} \)
(d) \( \ce{PO4^3-} \)
Show Answer & Explanation
Answer: (c) \( \ce{H2PO3-} \)
Explanation:
1. Add one proton to \( \ce{HPO3^2-} \) to get \( \ce{H2PO3-} \).
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) hydrogenation
(b) hydroxylation
(c) hydrolysis
(d) neutralisation
Show Answer & Explanation
Answer: (d) neutralisation
Explanation:
1. \( \ce{H+ + OH- -> H2O} \) is neutralisation.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) acid B
(b) acid A
(c) both A and B
(d) neither A nor B
Show Answer & Explanation
Answer: (a) acid B
Explanation:
1. A smaller pKa means a larger \( K_a \) and a stronger acid, so B is stronger.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) a strong acid and a strong base
(b) a strong acid and a weak base
(c) a weak acid and a weak base
(d) a weak acid and a strong base
Show Answer & Explanation
Answer: (d) a weak acid and a strong base
Explanation:
1. The anion of the weak acid hydrolyses and produces \( \ce{OH-} \).
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{NaH2PO2} \)
(b) \( \ce{NaH2PO3} \)
(c) \( \ce{NaH2PO4} \)
(d) None of these
Show Answer & Explanation
Answer: (a) \( \ce{NaH2PO2} \)
Explanation:
1. \( \ce{H3PO2} \) is monobasic, so \( \ce{NaH2PO2} \) is a normal salt with no replaceable hydrogen.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) weakly acidic
(b) weakly basic
(c) strongly acidic
(d) neither acidic nor basic
Show Answer & Explanation
Answer: (b) weakly basic
Explanation:
1. Carbonate ion is hydrolysed more strongly than ammonium ion (Kb of \( \ce{CO3^2-} \) exceeds Ka of \( \ce{NH4+} \)), so the solution is weakly basic.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) acidic
(b) basic
(c) neutral
(d) slightly basic
Show Answer & Explanation
Answer: (a) acidic
Explanation:
1. \( \ce{H+} \) = 2 \( \times \) 0.02 = 0.04 mol; \( \ce{OH-} \) = 0.02 mol.
2. Excess \( \ce{H+} \) remains, so the solution is acidic.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) monobasic and a weak Lewis acid
(b) monobasic and a weak Bronsted acid
(c) monobasic and a strong Lewis acid
(d) tribasic and a weak Bronsted acid
Show Answer & Explanation
Answer: (a) monobasic and a weak Lewis acid
Explanation:
1. Boric acid accepts \( \ce{OH-} \) from water: \( \ce{B(OH)3 + H2O -> [B(OH)4]- + H+} \).
2. It is monobasic and acts as a weak Lewis acid.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{CO2} \)
(b) \( \ce{SO3} \)
(c) \( \ce{SO2} \)
(d) \( \ce{ROH} \)
Show Answer & Explanation
Answer: (d) \( \ce{ROH} \)
Explanation:
1. An alcohol has lone pairs on oxygen and donates them; the oxides are electron acceptors.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) 10 mL of 1 M NaOH
(b) 10 mL of 2 M NaOH
(c) 5 mL of 2 M KOH
(d) 5 mL of 1 M \( \ce{Na2CO3} \)
Show Answer & Explanation
Answer: (b) 10 mL of 2 M NaOH
Explanation:
1. \( \ce{H2SO4} \) gives 20 mmol of \( \ce{H+} \).
2. 10 mL of 2 M NaOH gives 20 mmol of \( \ce{OH-} \).
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) acidic
(b) alkaline
(c) neutral
(d) strongly alkaline
Show Answer & Explanation
Answer: (a) acidic
Explanation:
1. NaOH = 100 mmol, giving 100 mmol of \( \ce{OH-} \).
2. Acid = 100 mmol, giving 200 mmol of \( \ce{H+} \).
3. Excess \( \ce{H+} \) makes it acidic.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) salts of strong acids and strong bases
(b) salts of weak acids and weak bases
(c) either weak acids or weak bases
(d) either strong acids or strong bases
Show Answer & Explanation
Answer: (c) either weak acids or weak bases
Explanation:
1. Indicators are weak organic acids or bases whose ionised and unionised forms have different colours.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) turn red litmus blue
(b) turn blue litmus red
(c) not affect litmus
(d) decolourise litmus
Show Answer & Explanation
Answer: (a) turn red litmus blue
Explanation:
1. Acetate ion hydrolyses to give \( \ce{OH-} \), so the solution is basic.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{HClO4} \)
(b) \( \ce{HCl} \)
(c) \( \ce{HOCl} \)
(d) \( \ce{HClO3} \)
Show Answer & Explanation
Answer: (b) \( \ce{HCl} \)
Explanation:
1. Removing a proton from HCl gives \( \ce{Cl-} \).
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) strong acid
(b) weak acid
(c) strong base
(d) weak base
Show Answer & Explanation
Answer: (b) weak acid
Explanation:
1. A strong base has a very strong tendency to accept protons, so its conjugate acid holds on to the proton and is a very weak acid.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{HNO3} \)
(b) \( \ce{HClO4} \)
(c) \( \ce{H2SO4} \)
(d) \( \ce{HBr} \)
Show Answer & Explanation
Answer: (a) \( \ce{HNO3} \)
Explanation:
1. All four are strong acids; the order of strength is \( \ce{HClO4} \) > HBr > \( \ce{H2SO4} \) > \( \ce{HNO3} \).
2. So \( \ce{HNO3} \) is the weakest.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{PO4^3-} \)
(b) \( \ce{H2PO4-} \)
(c) \( \ce{H3PO4} \)
(d) \( \ce{H4PO3} \)
Show Answer & Explanation
Answer: (a) \( \ce{PO4^3-} \)
Explanation:
1. Remove one proton from \( \ce{HPO4^2-} \): \( \ce{PO4^3-} \).
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) both correct
(b) both wrong
(c) (i) correct and (ii) wrong
(d) (i) wrong and (ii) correct
Show Answer & Explanation
Answer: (a) both correct
Explanation:
1. (i) is correct: the conjugate base of a strong acid is a very weak base.
2. (ii) is the Lewis definition of an acid, so it is also correct.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{FeCl3} \)
(b) \( \ce{NaCN} \)
(c) \( \ce{NaOH} \)
(d) \( \ce{NaCl} \)
Show Answer & Explanation
Answer: (a) \( \ce{FeCl3} \)
Explanation:
1. \( \ce{Fe^3+} \) is hydrolysed to give \( \ce{H+} \), so the solution of \( \ce{FeCl3} \) is acidic.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
(a) \( \ce{I2} \)
(b) \( \ce{I-} \)
(c) \( \ce{I3-} \)
(d) none of these
Show Answer & Explanation
Answer: (b) \( \ce{I-} \)
Explanation:
1. \( \ce{I-} \) donates a lone pair to \( \ce{I2} \), so it is the Lewis base.
Teacher's Note:
1. Recall the definition (Arrhenius, Bronsted-Lowry or Lewis) that the question is based on.
2. For a conjugate pair, add or remove one proton; a strong acid has a weak conjugate base.
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Equilibrium Objective Questions & Solutions for JEE Chemistry
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FAQs
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