Final answer:
The calculation of the solubility product for sparingly soluble salts involves writing the dissolution equation, determining molar solubility from the given solubility data, and applying stoichiometry to find the product of the ions' concentrations at equilibrium, hence obtaining the Ksp value.
Step-by-step explanation:
The question pertains to the calculation of the solubility product (Ksp) for various sparingly soluble salts based on their given solubility in water.
To calculate the solubility product, we must write the dissolution equation for each salt, determine the molar solubility from the given solubility in grams per 100 mL, and then use the stoichiometry of the dissolution to find the concentrations of the ions at equilibrium.
The product of these concentrations, each raised to the power of their respective stoichiometric coefficients, gives the Ksp of the salt.
For example, if a salt AB dissociates in water as AB(s) → A⁺(aq) + B⁻(aq), and its given solubility is 's' mol/L, the solubility product Ksp would be calculated as Ksp = [A⁺]²[B⁻]² = s².