Questions on Solubility Product Constant (Ksp)
Multiple-Choice Questions: Solubility Product Constant (Ksp)
1. What does the solubility product constant (Ksp) represent?
A) The amount of solute dissolved at any temperature
B) The product of the concentrations of the ions raised to the power of their coefficients
C) The speed at which a solute dissolves
D) The concentration of a saturated solution
E) The total number of ions formed
2. Which of the following salts has the simplest Ksp expression?
A) CaF₂
B) Fe(OH)₃
C) Ag₂CrO₄
D) NaCl
E) BaSO₄
3. The Ksp expression for PbCl₂ is:
A) [Pb²⁺][Cl⁻]
B) [Pb²⁺]²[Cl⁻]
C) [Pb²⁺][Cl⁻]²
D) [Pb⁴⁺][Cl⁻]²
E) [Pb⁺][Cl⁻]³
4. For the dissociation: Ag₂CO₃ ⇌ 2Ag⁺ + CO₃²⁻, what is the correct Ksp expression?
A) [Ag⁺][CO₃²⁻]
B) [Ag⁺]²[CO₃²⁻]
C) 2[Ag⁺][CO₃²⁻]²
D) [Ag₂CO₃]/[CO₃²⁻]
E) [CO₃²⁻]²/[Ag⁺]²
5. If the Ksp of CaF₂ is 3.9 × 10⁻¹¹, what is its molar solubility (s)?
A) 1.0 × 10⁻⁴ M
B) 2.5 × 10⁻⁴ M
C) 1.4 × 10⁻³ M
D) 3.3 × 10⁻⁴ M
E) 6.5 × 10⁻⁶ M
6. What is the molar solubility of Ag₂SO₄ if Ksp = 1.2 × 10⁻⁵?
A) 1.1 × 10⁻² M
B) 1.5 × 10⁻² M
C) 8.2 × 10⁻³ M
D) 1.8 × 10⁻² M
E) 7.0 × 10⁻³ M
7. Which factor does NOT affect the Ksp value?
A) Temperature
B) Presence of common ions
C) Type of solvent
D) Ionic strength
E) Pressure (for solids)
8. If solubility of BaF₂ is 1.0 × 10⁻³ M, what is its Ksp?
A) 4.0 × 10⁻⁹
B) 2.5 × 10⁻¹⁰
C) 1.0 × 10⁻⁶
D) 2.0 × 10⁻⁷
E) 3.2 × 10⁻¹¹
9. The common ion effect will:
A) Increase the solubility of a salt
B) Have no effect on solubility
C) Decrease the solubility of a salt
D) Change the Ksp
E) Remove the precipitate
10. What happens to solubility if you add NaCl to a solution of AgCl?
A) Solubility increases
B) Ksp increases
C) Solubility decreases
D) No change
E) Reaction stops
11. Which of the following will precipitate first when mixing with NaCl?
A) AgCl (Ksp = 1.8 × 10⁻¹⁰)
B) PbCl₂ (Ksp = 1.7 × 10⁻⁵)
C) Hg₂Cl₂ (Ksp = 1.3 × 10⁻¹⁸)
D) CuCl (Ksp = 1.9 × 10⁻⁷)
E) BaCl₂ (soluble)
12. A salt has Ksp = 2.5 × 10⁻⁸ and dissolves as AB₂. What is the molar solubility?
A) 1.3 × 10⁻³ M
B) 1.9 × 10⁻³ M
C) 1.7 × 10⁻² M
D) 2.4 × 10⁻⁴ M
E) 2.9 × 10⁻³ M
13. If the solubility of Mg(OH)₂ is s, the Ksp is expressed as:
A) s²
B) s³
C) 2s³
D) 4s³
E) s × 2s²
14. What is the solubility of PbBr₂ if Ksp = 6.3 × 10⁻⁶?
A) 9.5 × 10⁻³ M
B) 1.2 × 10⁻² M
C) 1.6 × 10⁻² M
D) 1.4 × 10⁻² M
E) 8.6 × 10⁻³ M
15. Which salt is least soluble in water based on Ksp values?
A) AgCl (Ksp = 1.8 × 10⁻¹⁰)
B) PbBr₂ (Ksp = 6.3 × 10⁻⁶)
C) CaF₂ (Ksp = 3.9 × 10⁻¹¹)
D) BaSO₄ (Ksp = 1.1 × 10⁻¹⁰)
E) Hg₂Cl₂ (Ksp = 1.3 × 10⁻¹⁸)
16. If the solubility of Al(OH)₃ is s, the Ksp expression is:
A) s²
B) 3s²
C) 4s³
D) 27s⁴
E) s³
17. What does a low Ksp value imply?
A) High solubility
B) Fast reaction
C) Low solubility
D) Strong acid
E) Common ion present
18. Which compound has a 1:1 ion ratio?
A) PbCl₂
B) CaF₂
C) Na₂SO₄
D) BaSO₄
E) Ag₂CrO₄
19. What is the effect of increasing temperature on the solubility of most salts?
A) No change
B) Decrease solubility
C) Increase solubility
D) Precipitation occurs
E) Reacts with water
20. Which salt will remain in solution if [Cl⁻] = 1.0 × 10⁻³ M?
A) AgCl (Ksp = 1.8 × 10⁻¹⁰)
B) PbCl₂ (Ksp = 1.7 × 10⁻⁵)
C) Hg₂Cl₂ (Ksp = 1.3 × 10⁻¹⁸)
D) CuCl (Ksp = 1.9 × 10⁻⁷)
E) All will precipitate
- Questions on Nonreversible Reactions
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Answer Key with Explanations
1. B – Ksp is the product of ion concentrations, each raised to their stoichiometric coefficients.
2. D – NaCl dissociates into 1:1 ions, so Ksp = [Na⁺][Cl⁻], simplest form.
3. C – PbCl₂ → Pb²⁺ + 2Cl⁻ → Ksp = [Pb²⁺][Cl⁻]²
4. B – Ag₂CO₃ → 2Ag⁺ + CO₃²⁻ → Ksp = [Ag⁺]²[CO₃²⁻]
5. D – Use Ksp = [Ca²⁺][F⁻]² = s × (2s)² = 4s³ → solve for s
6. E – Ag₂SO₄ → 2Ag⁺ + SO₄²⁻ → Ksp = 4s³ → solve for s
7. B – The common ion doesn’t affect Ksp, only solubility
8. A – BaF₂ → Ba²⁺ + 2F⁻ → Ksp = s × (2s)² = 4s³ = 4×10⁻⁹
9. C – The common ion effect reduces solubility
10. C – Cl⁻ is a common ion for AgCl, reducing its solubility
11. C – Hg₂Cl₂ has the lowest Ksp, precipitates first
12. A – AB₂ → A²⁺ + 2B⁻ → Ksp = 4s³ → solve for s
13. D – Mg(OH)₂ → Mg²⁺ + 2OH⁻ → Ksp = s × (2s)² = 4s³
14. A – PbBr₂ → Pb²⁺ + 2Br⁻ → Ksp = s × (2s)² = 4s³ → solve for s
15. E – The lower the Ksp, the less soluble → Hg₂Cl₂
16. D – Al(OH)₃ → Al³⁺ + 3OH⁻ → Ksp = s × (3s)³ = 27s⁴
17. C – Low Ksp = poorly soluble
18. D – BaSO₄ dissociates into Ba²⁺ + SO₄²⁻ (1:1 ratio)
19. C – Most salts are more soluble at higher temperatures
20. B – Only PbCl₂ has high enough Ksp to remain dissolved at [Cl⁻] = 10⁻³ M
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