The Solubility Product Constant (17.4.1)

Question 1

• Ksp is the solubility product constant, which governs the equilibria of sparingly soluble salts. Given AxBy(s) = xA+(aq) + yB–(aq), Ksp = [A+]^x[B–]^y.

Answer 1

• Ksp is the solubility product constant, which governs the equilibria of sparingly soluble salts. Given AxBy(s) = xA+(aq) + yB–(aq), Ksp = [A+]^x[B–]^y.

Question 2

• Solids do not appear in solubility product equations because they have a fixed value.

Answer 2

• Solids do not appear in solubility product equations because they have a fixed value.

Question 3

• The concentrations of individual ions are taken to the power of their stoichiometric coefficients in the Ksp equation.

Answer 3

• The concentrations of individual ions are taken to the power of their stoichiometric coefficients in the Ksp equation.

Question 4

• If the concentrations of the ions in a saturated solution are known, the Ksp can be calculated.

Answer 4

• If the concentrations of the ions in a saturated solution are known, the Ksp can be calculated.