AP®ChemistryCollege BoardExam QuestionsUnit 7: EquilibriumSolubility Equilibria

Solubility Equilibria (College Board AP® Chemistry): Exam Questions

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Solubility Equilibria

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11 mark

The correct form of the solubility product for calcium phosphate, Ca3(PO4)2, is

  • [Ca2+][PO43–]

  • [Ca2+]2[PO43–]3

  • [Ca2+]3[PO43–]2

  • [Ca2+]3[PO3–]4

Choose your answer

21 mark

For the following reaction at equilibrium

H2S (aq)  +  Mg2+ (aq)  ⇋   MgS (s)   +  2H+ (aq)              ΔH < 0

The reaction occurs in an aqueous solution, and MgS precipitates as a solid.

Which of the following changes will result in more MgS being produced?

  • Adding sodium hydroxide.

  • Decreasing the pressure.

  • Adding H⁺ ions.

  • Increasing the temperature.

Choose your answer

11 mark

Ca(NO3)2 + K2SO4 → CaSO4 + 2KNO3

Ksp = 2.00 x 10-5 at 298 K

100 mL of a 1.70 x 10-3 M solution of calcium nitrate is slowly added to 100 mL of 1.50 x 10-3 M potassium sulfate.

Which of the following will be observed?

  • A precipitate forms because Q > Ksp

  • A precipitate forms because Q < Ksp

  • No precipitate forms because Q > Ksp

  • No precipitate forms because Q < Ksp

Choose your answer

11 mark

A saturated solution of Sr(OH)2 has a pH of 12.50. What is the solubility product of Sr(OH)2?

  • 3.28 x 10-5

  • 1.64 x 10-5

  • 1.58 x 10-38

  • 5.12 x 10-4

Choose your answer

21 mark

The solubility of silver carbonate (Ag2CO3) in pure water at 25∘C is found to be 8.45×10−3 M. If 0.100 M of sodium carbonate (Na2CO3) is added to the solution, what is the new solubility of Ag2CO3 assuming the solution reaches equilibrium?
The Ksp of Ag2CO3 at 25∘C is 8.1×10−12.

  • 8.1×10−10 M

  • 8.1×10−8 M

  • 8.1×10−6 M

  • 8.1×10−5 M

Choose your answer