Write the solubility product expression, Ksp, for a slightly
soluble ionic compound.
Calculate Ksp from the solubility of ionic compound or solubility
from the value of Ksp.
Calculate the effect of common ions on the aqueous solubilities of sparingly
soluble salts.
Determine if a salt will precipitate from solution based on the
concentrations of its ions.
Determine the concentration of ions remaining in solution after
precipitation and predict whether precipitation will be complete.
Explain how fractional precipitation works and when it can be used.
Describe, through net ionic equations and calculations, the effect of pH on
the precipitation and dissolving of certain substances.
Write equations showing the effect of complex ion formation on other
equilibrium processes such as solubility equilibria.
Use complex ion formation constants, Kf (from table 19-2 or Appendix
D in the text), to compute the concentrations in solution of: free
ions, ligands, and complex ions.
Use Kf values along with Ksp values to determine the
solubilities of slightly soluble solutes in the presence of complexing
ligands.
Calculate the solubilities of certain solutes in the presence of complexing
ligands.