Final answer:
The dissolution equations and solubility product expressions for BaSO4, Ca(OH)2, Ag2CO3, and PbCl2 are provided, showing the dissociation of each compound into its ions and the respective Ksp equations.
Step-by-step explanation:
To write the ionic equations for the dissolution and the solubility product (Ksp) expressions for the given slightly soluble ionic compounds, we consider the ions they dissociate into and the stoichiometry of the resulting equilibrium:
BaSO4 (s) → Ba2+ (aq) + SO42- (aq)
Ksp = [Ba2+][SO42-]
Ca(OH)2 (s) → Ca2+ (aq) + 2 OH- (aq)
Ksp = [Ca2+][OH-]2
Ag2CO3 (s) → 2 Ag+ (aq) + CO32- (aq)
Ksp = [Ag+]2[CO32-]
PbCl2 (s) → Pb2+ (aq) + 2 Cl- (aq)
Ksp = [Pb2+][Cl-]2
The ionic equations show how each solid dissociates into its component ions when it dissolves. The solubility product expressions provide a way of calculating the equilibrium concentration of these ions in solution at saturation.