JEE Chemistry Ionic Equilibrium MCQs Set 34

Download JEE MCQs for JEE Chemistry: Ionic Equilibrium

Review structured MCQ sets for JEE Chemistry Ionic Equilibrium. Built according to official JEE guidelines, these downloadable questions support daily revision and core concept reinforcement.

Chapter-wise Objective Questions: Ionic Equilibrium

Access the complete set of multiple-choice questions for Ionic Equilibrium below. This focused format allows students to isolate specific topics for thorough review and uninterrupted practice alongside official JEE textbooks.

Multiple Choice Questions

Question 1: What is the expression for Ksp of PbCl2?
(a) [Pb2+][2Cl−]2
(b) [Pb+]/[2Cl−]2
(c) [Pb2+][Cl−]2
(d) [Pb2+]/[Cl−]2
Show Answer & Explanation

Answer: (c) [Pb2+][Cl−]2

Explanation:
1. PbCl2 ⇌ Pb2+ + 2Cl−.
2. The coefficient becomes an exponent: Ksp = [Pb2+][Cl−]2.
3. Answer: (c)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 2: At 25°C, the solubility product of Hg2Cl2 in water is 3.2 × 10−17 mol3 dm−9. What is the solubility of Hg2Cl2 in water at 25°C?
(a) 1.2 × 10−12 M
(b) 3.0 × 10−6 M
(c) 2 × 10−6 M
(d) 1.2 × 10−16 M
Show Answer & Explanation

Answer: (c) 2 × 10−6 M

Explanation:
1. Hg2Cl2 ⇌ Hg22+ + 2Cl−, so Ksp = s(2s)2 = 4s3.
2. s3 = 8 × 10−18, so s = 2 × 10−6 M.
3. Answer: (c)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 3: When a buffer solution of CH3COOH and CH3COONa is diluted with water (the ratio [salt]/[acid] stays constant):
(a) CH3COO− ion concentration increases
(b) H+ ion concentration increases
(c) OH− ion concentration increases
(d) H+ ion concentration does not change
Show Answer & Explanation

Answer: (d) H+ ion concentration does not change

Explanation:
1. [H+] = Ka[acid]/[salt].
2. Both concentrations fall by the same factor on dilution, so the ratio and the pH stay the same.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 4: The solubility products of AgCl and AgI are 1.1 × 10−10 and 1.6 × 10−16 respectively. If AgNO3 is added drop by drop to a solution containing both chloride and iodide ions, which salt will precipitate first?
(a) AgI
(b) AgNO3
(c) AgCl
(d) Both AgCl and AgI simultaneously
Show Answer & Explanation

Answer: (a) AgI

Explanation:
1. The salt needing the smaller [Ag+] precipitates first.
2. For equal anion concentrations that is AgI, with the much smaller Ksp.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 5: Which one of the following is an acidic salt?
(a) Na2HPO3
(b) NH4NO3
(c) NaH2PO2
(d) NaHCO3
Show Answer & Explanation

Answer: (d) NaHCO3

Explanation:
1. An acid salt still contains an ionisable hydrogen from an incompletely neutralised acid, and NaHCO3 retains one from H2CO3.
2. H3PO3 is dibasic and H3PO2 is monobasic, so Na2HPO3 and NaH2PO2 are normal salts; NH4NO3 is also a normal salt.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 6: Which of the following is the conjugate base of OH−?
(a) O2−
(b) O−
(c) H2O
(d) O2
Show Answer & Explanation

Answer: (a) O2−

Explanation:
1. The conjugate base is formed by removing one H+.
2. OH− − H+ = O2−.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 7: CH3NH2 (0.1 mole, Kb = 5 × 10−4) is added to 0.08 mole of HCl and the solution is diluted to one litre. The resulting hydrogen ion concentration is:
(a) 1.6 × 10−11
(b) 8 × 10−11
(c) 5 × 10−5
(d) 8 × 10−2
Show Answer & Explanation

Answer: (b) 8 × 10−11

Explanation:
1. Left: 0.02 mol base and 0.08 mol CH3NH3Cl, a basic buffer.
2. [OH−] = Kb × 0.02/0.08 = 1.25 × 10−4 M.
3. [H+] = 10−14/1.25 × 10−4 = 8 × 10−11 M.
4. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 8: If Na2CO3 is added to a solution of H2CO3, the pH of the H2CO3 solution:
(a) decreases
(b) remains constant
(c) increases
(d) cannot be predicted
Show Answer & Explanation

Answer: (c) increases

Explanation:
1. CO32− is a common ion with the second ionisation and also a base.
2. It suppresses ionisation and consumes H+, so the pH increases.
3. Answer: (c)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 9: Calculate the pH of a solution containing 0.1 M CH3COOH and 0.15 M CH3COO− (Ka of CH3COOH = 1.8 × 10−5).
(a) 9.1
(b) 3.9
(c) 10
(d) 4.91
Show Answer & Explanation

Answer: (d) 4.91

Explanation:
1. pH = pKa + log([salt]/[acid]).
2. = 4.74 + log 1.5 = 4.74 + 0.18 = 4.92 ≈ 4.91.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 10: In a saturated aqueous solution of AgBr, the concentration of Ag+ is 1 × 10−6 mol L−1. If Ksp of AgBr is 4 × 10−13, the Br− concentration in the solution is:
(a) 1 × 10−6 mol L−1
(b) 4 × 10−8 mol L−1
(c) 4 × 10−7 mol L−1
(d) 4 × 10−19 mol L−1
Show Answer & Explanation

Answer: (c) 4 × 10−7 mol L−1

Explanation:
1. [Br−] = Ksp/[Ag+].
2. = 4 × 10−13/10−6 = 4 × 10−7 mol L−1 (Ag+ exceeds √Ksp here, so some Ag+ comes from another source).
3. Answer: (c)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 11: A solution of an acid has pH = 4.70. Find the concentration of OH− ions (pKw = 14).
(a) 5 × 10−10
(b) 6 × 10−10
(c) 2 × 10−6
(d) 9 × 10−6
Show Answer & Explanation

Answer: (a) 5 × 10−10

Explanation:
1. pOH = 14 − 4.70 = 9.30.
2. [OH−] = 10−9.3 = 5.0 × 10−10 M.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 12: Which of the following is NOT an example of a buffer solution?
(a) HNO2 + KNO2
(b) HF + KF
(c) PhNH2 + PhNH3+Cl−
(d) NH4Cl + HCl
Show Answer & Explanation

Answer: (d) NH4Cl + HCl

Explanation:
1. A buffer needs a weak acid with its conjugate base, or a weak base with its conjugate acid.
2. NH4Cl + HCl is a salt of a weak base plus a strong acid, so there is no weak base to take up H+.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 13: Which of the following acids will release the maximum amount of heat when completely neutralised by the strong base NaOH?
(a) 1 M HCl
(b) 1 M HNO3
(c) 1 M HClO4
(d) 1 M H2SO4
Show Answer & Explanation

Answer: (d) 1 M H2SO4

Explanation:
1. Each strong acid releases about 57 kJ per mole of H+ neutralised.
2. 1 M H2SO4 supplies 2 mol H+ per litre, so it gives double the heat.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 14: Which of the following is an example of a hydrolysis reaction?
(a) NH4Cl ⇌ NH4+ + Cl−
(b) NH4+ + H2O ⇌ NH4OH + H+
(c) Na+ + H2O ⇌ NaOH + H+
(d) CH3COOH + HOC2H5 ⇌ CH3COOC2H5 + H2O
Show Answer & Explanation

Answer: (b) NH4+ + H2O ⇌ NH4OH + H+

Explanation:
1. Hydrolysis is the reaction of an ion of a salt with water.
2. NH4+ reacts with water giving NH4OH and H+; Na+ (from a strong base) does not hydrolyse.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 15: Which of the following salts will have the lowest pH in water of equal molarity?
(a) Na2SO4
(b) (NH4)2SO4
(c) Na2CO3
(d) NaCl
Show Answer & Explanation

Answer: (b) (NH4)2SO4

Explanation:
1. Na2SO4 and NaCl are neutral, Na2CO3 is basic.
2. (NH4)2SO4 is a weak base-strong acid salt and is acidic, so it has the lowest pH.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 16: What will be the pH of 0.1 M NaCN solution if Ka for HCN is 10−6 at 25°C?
(a) 6.5
(b) 9.5
(c) 3
(d) 7
Show Answer & Explanation

Answer: (b) 9.5

Explanation:
1. Kh = Kw/Ka = 10−8.
2. [OH−] = √(KhC) = √(10−9) = 3.16 × 10−5, so pOH = 4.5 and pH = 9.5.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 17: The conjugate base of the strong acid in the reaction CH3COOH + HCl ⇌ Cl− + CH3COOH2+ will be:
(a) HCl
(b) Cl−
(c) CH3COOH
(d) CH3COOH2+
Show Answer & Explanation

Answer: (b) Cl−

Explanation:
1. HCl donates a proton and is the stronger acid here.
2. Its conjugate base is Cl−.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 18: What will be the approximate degree of dissociation of a 0.005 M NH4OH solution if pKb for NH4OH is 4.7?
(a) 2%
(b) 0.03%
(c) 0.40%
(d) 6.32%
Show Answer & Explanation

Answer: (d) 6.32%

Explanation:
1. Kb = 10−4.7 = 2 × 10−5.
2. α = √(Kb/C) = √(2 × 10−5/0.005) = 0.0632 = 6.32%.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 19: Which of the following pairs can be used to form a buffer solution?
(a) H2SO4 and Na2SO4
(b) NaOCl and NaCl
(c) NH3 and NH4Cl
(d) NaH2PO4 and NaCl
Show Answer & Explanation

Answer: (c) NH3 and NH4Cl

Explanation:
1. A basic buffer is a weak base with a salt of its conjugate acid.
2. NH3 and NH4Cl fit; H2SO4 is a strong acid and NaCl is a neutral salt.
3. Answer: (c)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 20: What is the molar solubility of MgF2 in a 0.2 M solution of KF? (Ksp = 8 × 10−8)
(a) 8 × 10−8 M
(b) 8 × 10−7 M
(c) 2 × 10−6 M
(d) 2.7 × 10−4 M
Show Answer & Explanation

Answer: (c) 2 × 10−6 M

Explanation:
1. [F−] ≈ 0.2 M from KF.
2. s = [Mg2+] = Ksp/(0.2)2 = 8 × 10−8/0.04 = 2 × 10−6 M.
3. Answer: (c)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 21: If pKa of acetic acid and pKb of ammonium hydroxide are 4.76 each, the pH of ammonium acetate at 25°C is:
(a) 7
(b) less than 7
(c) more than 7
(d) 0
Show Answer & Explanation

Answer: (a) 7

Explanation:
1. pH = 7 + ½(pKa − pKb) = 7 + 0 = 7.
2. Equal strengths of acid and base give a neutral solution.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 22: What is the hydronium ion concentration of 0.25 M HA solution? (Ka = 4 × 10−8)
(a) 10−4
(b) 10−5
(c) 10−7
(d) 10−10
Show Answer & Explanation

Answer: (a) 10−4

Explanation:
1. [H3O+] = √(KaC) = √(4 × 10−8 × 0.25).
2. = √(10−8) = 10−4 M.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 23: The solubility of PbF2 (molecular weight 245) is 0.46 g/L. What is its solubility product?
(a) 1.1 × 10−10
(b) 2.6 × 10−8
(c) 1.1 × 10−7
(d) 6.8 × 10−9
Show Answer & Explanation

Answer: (b) 2.6 × 10−8

Explanation:
1. s = 0.46/245 = 1.88 × 10−3 mol L−1.
2. Ksp = 4s3 = 4 × (1.88 × 10−3)3 = 2.6 × 10−8.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 24: What is the molar solubility of Ag2CO3 (Ksp = 4 × 10−13) in 0.1 M Na2CO3 solution?
(a) 10−6
(b) 10−7
(c) 2 × 10−6
(d) 2 × 10−7
Show Answer & Explanation

Answer: (a) 10−6

Explanation:
1. [CO32−] ≈ 0.1 M and [Ag+] = 2s.
2. (2s)2 × 0.1 = 4 × 10−13 gives s2 = 10−12, so s = 10−6 M.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 25: When 50 mL of 0.10 M ammonia solution is treated with 50 mL of 0.05 M HCl solution, the pH is (pKb of ammonia = 4.74):
(a) 8.26
(b) 9.26
(c) 4.74
(d) None of these
Show Answer & Explanation

Answer: (b) 9.26

Explanation:
1. NH3 = 5 mmol, HCl = 2.5 mmol, so 2.5 mmol NH3 and 2.5 mmol NH4+ remain.
2. The buffer is at half-neutralisation, so pOH = pKb = 4.74 and pH = 9.26.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 26: Which salt is most soluble?
(a) CaF2 (Ksp = 5.3 × 10−9)
(b) BaCrO4 (Ksp = 1.2 × 10−10)
(c) CaC2O4 (Ksp = 4 × 10−9)
(d) Hg2Cl2 (Ksp = 1.3 × 10−18)
Show Answer & Explanation

Answer: (a) CaF2 (Ksp = 5.3 × 10−9)

Explanation:
1. Molar solubilities: CaF2 (4s3) = 1.1 × 10−3 M; BaCrO4 = 1.1 × 10−5 M; CaC2O4 = 6.3 × 10−5 M; Hg2Cl2 (4s3) = 6.9 × 10−7 M.
2. CaF2 is the largest.
3. Answer: (a)

Teacher's Note:
1. Compare molar solubilities, not Ksp values, when salts have different formula types. Use s = (Ksp/4)1/3 for AB2 salts.

Question 27: Molar solubility of Cd(OH)2 (Ksp = 2.5 × 10−14) in 0.1 M KOH solution is:
(a) 2.5 × 10−7 M
(b) 5 × 10−8 M
(c) 5 × 10−7 M
(d) 2.5 × 10−12 M
Show Answer & Explanation

Answer: (d) 2.5 × 10−12 M

Explanation:
1. [OH−] ≈ 0.1 M from KOH.
2. s = Ksp/(0.1)2 = 2.5 × 10−14/10−2 = 2.5 × 10−12 M.
3. Answer: (d)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 28: What is [NH4+] in a solution that is 0.02 M NH3 and 0.01 M KOH? [Kb(NH3) = 1.8 × 10−5]
(a) 3.6 × 10−5 M
(b) 1.8 × 10−5 M
(c) 0.9 × 10−5 M
(d) 7.2 × 10−5 M
Show Answer & Explanation

Answer: (a) 3.6 × 10−5 M

Explanation:
1. KOH fixes [OH−] ≈ 0.01 M.
2. [NH4+] = Kb[NH3]/[OH−] = 1.8 × 10−5 × 0.02/0.01 = 3.6 × 10−5 M.
3. Answer: (a)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

Question 29: Which of the following has the maximum pH?
(a) 1 M H2S
(b) 1 M H2O
(c) 1 M H2Se
(d) 1 M H2Te
Show Answer & Explanation

Answer: (b) 1 M H2O

Explanation:
1. H2S, H2Se and H2Te are all acids (acidity increases down the group).
2. Water is neutral, so it has the highest pH of the four.
3. Answer: (b)

Teacher's Note:
1. Write the governing relation first, then substitute. Check that the final value is reasonable.

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Multiple Choice Questions (MCQs) for JEE Chemistry Ionic Equilibrium

About Ionic Equilibrium MCQs for JEE Chemistry

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