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Solubility product constant (Ksp) Knowledge-Based Practice

Chemistry · Chemical Equilibrium · Chemistry · Solubility Equilibria

5 Chemistry practice questions on Solubility product constant (Ksp). Questions that assess core concepts and understanding.

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Questions

  1. 1.

    The solubility product constant (KspK_{\text{sp}}) of silver chromate, Ag2CrO4\text{Ag}_2\text{CrO}_4, is 4.0×10−124.0 \times 10^{-12} at 25 °C. What is the concentration of Ag+\text{Ag}^+ ions in a saturated aqueous solution of Ag2CrO4\text{Ag}_2\text{CrO}_4 at this temperature?

    • A) 1.0×10−4 mol/L1.0 \times 10^{-4}\text{ mol/L}
    • B) 1.4×10−4 mol/L1.4 \times 10^{-4}\text{ mol/L}
    • C) 2.0×10−4 mol/L2.0 \times 10^{-4}\text{ mol/L}
    • D) 2.0×10−6 mol/L2.0 \times 10^{-6}\text{ mol/L}
  2. 2.

    A solution contains 1.0×10−4 mol/L1.0 \times 10^{-4}\text{ mol/L} of Ag+\text{Ag}^+ ions and 2.0×10−3 mol/L2.0 \times 10^{-3}\text{ mol/L} of Cl−\text{Cl}^- ions at 25 °C. Given that KspK_{\text{sp}} for AgCl\text{AgCl} is 1.8×10−101.8 \times 10^{-10} at this temperature, which of the following correctly describes the state of the solution?

    • A) The solution is unsaturated and no precipitate forms because Qsp<KspQ_{\text{sp}} < K_{\text{sp}}.
    • B) The solution is supersaturated and a precipitate forms because Qsp>KspQ_{\text{sp}} > K_{\text{sp}}.
    • C) The solution is saturated and in dynamic equilibrium because Qsp=KspQ_{\text{sp}} = K_{\text{sp}}.
    • D) The solution is saturated and additional solid dissolves because Qsp>KspQ_{\text{sp}} > K_{\text{sp}}.
  3. 3.

    A solution has a barium ion concentration of 1.0×10−31.0 \times 10^{-3} mol/L. What is the minimum concentration of sulfate ions required to begin the precipitation of BaSO4\text{BaSO}_4 at 25 °C, given that the KspK_{\text{sp}} of BaSO4\text{BaSO}_4 is 1.1×10−101.1 \times 10^{-10}?

    • A) 1.1×10−131.1 \times 10^{-13} mol/L
    • B) 1.1×10−71.1 \times 10^{-7} mol/L
    • C) 1.0×10−51.0 \times 10^{-5} mol/L
    • D) 1.1×10−41.1 \times 10^{-4} mol/L
  4. 4.

    What is the molar solubility of silver chloride (AgCl\text{AgCl}) in a 0.10 mol/L NaCl\text{NaCl} solution at 25 °C? (The KspK_{sp} of AgCl\text{AgCl} at 25 °C is 1.8×10−101.8 \times 10^{-10}.)

    • A) 1.3×10−51.3 \times 10^{-5} mol/L
    • B) 1.8×10−111.8 \times 10^{-11} mol/L
    • C) 1.8×10−81.8 \times 10^{-8} mol/L
    • D) 1.8×10−91.8 \times 10^{-9} mol/L
  5. 5.

    The molar solubility of calcium fluoride (CaF2\text{CaF}_2) in pure water at 25 °C is 2.0×10−4 mol/L2.0 \times 10^{-4}\text{ mol/L}. What is the solubility product constant (KspK_{sp}) of CaF2\text{CaF}_2 at this temperature?

    • A) 8.0×10−128.0 \times 10^{-12}
    • B) 3.2×10−113.2 \times 10^{-11}
    • C) 1.6×10−111.6 \times 10^{-11}
    • D) 4.0×10−84.0 \times 10^{-8}

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