# Ksp Problem Set

This problem set was developed by S.E. Van Bramer for Chemistry 146 at Widener University.

1. Calculate the molar solubility and Ksp 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 Ksp 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 Ksp 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 Ksp 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.