Systems in Chemical Equilibrium Le Châtelier's Principle Part I. Determination of the Solubility Product (Ksp) for Lead(II) Chloride Consider the system in equilibrium below which involves the dissolution of a sparingly soluble ionic compound. PbCl2 Pb2) +2 Cl(aq) The equilibrium constant Ke for the system is given by the product of the molar concentration of the lead(II) ion cation and the square of the molar concentration of the chloride anion. Recall that solids are omitted from equilibrium constants. At a given temperature therefore, this product is a constant reflecting the maximum relative amounts of these species in aqueous solution. The equilibrium constant in the dissolution of an ionic substance is termed the solubility product Ksp. By determining the maximum molar concentrations of both species, you will determine the solubility product for lead(II) chloride at room temperature. 1. Add 3.0 mL of 0.30 M lead(II) nitrate to a clean test tube. 2. Add 5.0 mL of0.30 M HCI to a 10 mL graduated cylinder and incrementally add the acid to the lead solution in 1 mL increments to the lead nitrate solution until a noticeable amount of the while lead(lI) chloride precipitate is formed. 3. Determine the molar amounts of both Pb and Cr in the test tube. Show your calculations below