Solubility Equilibrium and Ksp Practice Problems
Answer Key for Solubility Equilibrium
1A, 2C, 3B, 4C, 5A, 6C, 7C, 8B, 9A, 10D, 11D, 12A, 13B, 14C, 15C, 16D, 17B
Detailed Solutions for Solubility Problems
Problem 1: Net Ionic Equation and Precipitation
1a. Net Ionic Equation:
Pb2+ + 2Cl- → PbCl2(s)
1b. Precipitation Calculation:
moles Pb2+ = (0.0150)(0.0500) = 0.00075
moles Cl- = (0.0350)(0.0850) = 0.002975
total volume = 0.0500 L
[Pb2+] = 0.00075 / 0.0500 = 0.0150 M
[Cl-] = 0.002975 / 0.0500 = 0.0595 M
Q = [Pb2+][Cl-]2 = (0.0150)(0.0595)2
Q = 5.3 × 10-5
Ksp = 1.6 × 10-5
Since Q > Ksp, a precipitate indeed forms.
Problem 2: Calculating Ksp for Silver Sulfate
2a. Ksp of Ag2SO4:
moles = mass / molar mass
moles = (7.2 × 10-4) / 311.8 = 2.31 × 10-6 mol
s = moles / volume
s = (2.31 × 10-6) / 0.0500 = 4.62... Continue reading "Solubility Equilibrium and Ksp Practice Problems" »
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