K_sp Problem Set

1. Calculate the molar solubility and K_sp for each of the following.
   1. 6.11*10^-4 g BaSO₄ dissolves in 250.0 mL of water at 25 °C
   2. 0.3295 g BaF₂ dissolves in 250.0 mL of water at 25 °C
   3. 4.807*10^-4 g AgCl dissolves in 250.0 mL of water at 25 °C
   4. 1.667 g CaF₂ dissolves in 100.0 L of water at 25 °C

2. Use the K_sp values calculated above to determine the mass of each that will dissolve in 2.0 L of deionized water.
   1. BaSO₄
   2. BaF₂
   3. AgCl
   4. CaF₂

3. Use the K_sp values calculated above to determine.
   1. The mass of BaSO₄ that will dissolve in 500 mL of 0.10 M sodium sulfate.
   2. The mass of BaF₂ that will dissolve in 250 mL of 0.10 M potassium fluoride.
   3. The mass of AgCl that will dissolve in 5.0 L of 10^-4 M lithium chloride.
   4. The mass of CaF₂ that will dissolve in 5000.0 L of 0.10 M potassium fluoride.

4. Use the K_sp values calculated in the previious problem set to determine the mass of precipitate formed and the concentration all ions remaining in soultion when:
   1. 50.0 mL of 0.10 M barium acetate is mixed with 100.0 mL of 0.10 M sodium sulfate.
   2. 100.0 mL of 0.15 M barium chlorate is mixed with 250.0 mL of 0.10 M potassium fluoride.
   3. 75.0 mL of 0.015 M silver nitrate is mixed with 1.0 L of 10^-4 M lithium chloride.
   4. 100 L of 0.50 M calcium chloride is mixed with 5000.0 L of 0.10 M potassium fluoride.

Scott Van Bramer
Department of Chemistry
Widener University
Chester, PA 19013

© copyright 1996, S.E. Van Bramer
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Last Updated: Monday, January 25, 1999 10:31:17 AM