The solubility-product constant (or simply solubility product) is the equilibrium constant expression for the equilibrium between a solid and an aqueous solution of its component ions. Solids do not appear in the equilibrium constant expression for heterogeneous equilibria. Therefore, Ksp is equal to the product of the concentrations of the ions raised to the power of their stoichiometric coefficients.
CxAy <--> xC + yA
Ksp = [C]^x [A]^y
HW: On a separate sheet of paper, complete the following problem.
Problem -
(a) Write the chemical equation for the addition of CaF2 to distilled water.
(b) Write the equation for Ksp for the addition of CaF2 to distilled water.
(c) The Ksp for CaF2 at 25 degrees C is 3.9 x 10^-11. What is the solubility of CaF2 in grams per liter?
(d) What affect would the addition of Ca(NO3)2 have on the reaction?
(e) What affect would the addition of HCl have on the reaction?
