Skip to main content
Back

Ksp quiz #1

Control buttons has been changed to "navigation" mode.
1/18

Terms in this set (18)

  • Salt A has a greater solubility in water than Salt B. What can be said about their Ksp values?
    Salt A has a larger Ksp value than Salt B, indicating it is more soluble in water.
  • What is the solubility of MgCO3 in water if the Ksp of MgCO3 is 3.5 × 10⁻⁸?
    The solubility of MgCO3 in water can be calculated using the Ksp expression: Ksp = [Mg²⁺][CO₃²⁻]. Since both ions are produced in a 1:1 ratio, solubility (s) = √Ksp = √(3.5 × 10⁻⁸) ≈ 1.87 × 10⁻⁴ M.
  • The solubility of Ag3PO4 in water at 25°C is 4.3 × 10⁻⁵ M. What is the Ksp for Ag3PO4?
    Ksp = [Ag⁺]³[PO₄³⁻]. For Ag3PO4, [Ag⁺] = 3s, [PO₄³⁻] = s. Ksp = (3 × 4.3 × 10⁻⁵)³ × (4.3 × 10⁻⁵) ≈ 2.1 × 10⁻¹².
  • The solubility of PbSO4 in water at 25°C is 7.9 × 10⁻³ M. What is the Ksp for PbSO4?
    Ksp = [Pb²⁺][SO₄²⁻]. Both ions are produced in a 1:1 ratio, so Ksp = (7.9 × 10⁻³)² ≈ 6.24 × 10⁻⁵.
  • What is the solubility of Cd3(PO4)2 in water if the Ksp of Cd3(PO4)2 is 2.5 × 10⁻³³?
    Let s = solubility. Ksp = [Cd²⁺]³[PO₄³⁻]² = (3s)³(2s)² = 27s³ × 4s² = 108s⁵. s = (Ksp/108)^(1/5) = (2.5 × 10⁻³³ / 108)^(1/5) ≈ 1.1 × 10⁻⁷ M.
  • The solubility of Ag2SO4 in water at 25°C is 0.0155 M. What is the Ksp for Ag2SO4?
    Ksp = [Ag⁺]²[SO₄²⁻]. [Ag⁺] = 2s, [SO₄²⁻] = s. Ksp = (2 × 0.0155)² × 0.0155 ≈ 7.44 × 10⁻⁶.
  • What is the correct expression for the solubility product constant (Ksp) of Zn3(PO4)2?
    Ksp = [Zn²⁺]³[PO₄³⁻]².
  • The solubility of lead(II) chloride (PbCl2) is 1.6 × 10⁻² M. What is the Ksp of PbCl2?
    Ksp = [Pb²⁺][Cl⁻]². [Pb²⁺] = s, [Cl⁻] = 2s. Ksp = (1.6 × 10⁻²) × (2 × 1.6 × 10⁻²)² ≈ 8.19 × 10⁻⁶.
  • What is the value of Q when the solution contains 2.50 × 10⁻³ M Mg²⁺ and 2.00 × 10⁻³ M CO₃²⁻?
    Q = [Mg²⁺][CO₃²⁻] = (2.50 × 10⁻³) × (2.00 × 10⁻³) = 5.00 × 10⁻⁶.
  • The Ksp of PbBr2 is 6.60 × 10⁻⁶. What is the molar solubility of PbBr2 in pure water?
    Ksp = [Pb²⁺][Br⁻]². Let s = solubility. [Pb²⁺] = s, [Br⁻] = 2s. Ksp = s × (2s)² = 4s³. s = (Ksp/4)^(1/3) = (6.60 × 10⁻⁶ / 4)^(1/3) ≈ 1.19 × 10⁻² M.
  • If Ksp = 7 × 10⁻⁷, what is the molar solubility of a salt that dissociates into one cation and one anion?
    For a salt AB: Ksp = s², so s = √(7 × 10⁻⁷) ≈ 8.37 × 10⁻⁴ M.
  • What is the solubility (g/L) of CaF2 salt that has Ksp = 5.21 × 10⁻⁶ at 25°C?
    Ksp = [Ca²⁺][F⁻]². Let s = molar solubility. [Ca²⁺] = s, [F⁻] = 2s. Ksp = s × (2s)² = 4s³. s = (Ksp/4)^(1/3) ≈ 1.08 × 10⁻² M. Multiply by molar mass of CaF2 (78.07 g/mol): 1.08 × 10⁻² × 78.07 ≈ 0.84 g/L.
  • Under what condition does the Ksp for PbI2 decrease?
    Ksp is a constant at a given temperature; it can only decrease if the temperature decreases.
  • What is the molar solubility of Fe(OH)2 at 25°C if Ksp of the compound is 7.9 × 10⁻¹⁶?
    Ksp = [Fe²⁺][OH⁻]². [Fe²⁺] = s, [OH⁻] = 2s. Ksp = s × (2s)² = 4s³. s = (Ksp/4)^(1/3) = (7.9 × 10⁻¹⁶ / 4)^(1/3) ≈ 5.8 × 10⁻⁶ M.
  • What is the molar solubility in water of Ag2CrO4? (The Ksp for Ag2CrO4 is 8 × 10⁻¹².)
    Ksp = [Ag⁺]²[CrO₄²⁻]. [Ag⁺] = 2s, [CrO₄²⁻] = s. Ksp = (2s)² × s = 4s³. s = (Ksp/4)^(1/3) = (8 × 10⁻¹² / 4)^(1/3) ≈ 1.26 × 10⁻⁴ M.
  • Enter the Ksp expression for the solid AB2 in terms of the molar solubility x.
    Ksp = [A²⁺][B⁻]² = x × (2x)² = 4x³.
  • The Ksp of PbBr2 is 6.60 × 10⁻⁶. What is the molar solubility of PbBr2?
    Let s = molar solubility. Ksp = 4s³, so s = (6.60 × 10⁻⁶ / 4)^(1/3) ≈ 1.19 × 10⁻² M.
  • Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4) = 1.82 × 10⁻⁸.
    Ksp = [Pb²⁺][SO₄²⁻] = s². s = √(1.82 × 10⁻⁸) ≈ 1.35 × 10⁻⁴ M.