Question: This is a 2 part question Part A. Part B. PbCl2(s)Pb2+(aq)+2Cl(aq) Suppose you add 0.2371g of PbCl2(s) to 50.0mL of water. When the solution reaches

This is a 2 part question

Part A. This is a 2 part question Part A. Part B. PbCl2(s)Pb2+(aq)+2Cl(aq)

Part B. Suppose you add 0.2371g of PbCl2(s) to 50.0mL of water. When the

PbCl2(s)Pb2+(aq)+2Cl(aq) Suppose you add 0.2371g of PbCl2(s) to 50.0mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+(aq) is 0.0159M and the concentration of Cl(aq) is 0.0318M. What is the value of the equilibrium constant, Ksp,, for the dissolution of PbCl2 ? (Note that the equilibrium constant associated with sparingly soluble salts is called the solubility product constant, Ksp..) Using the procedure in Determination of an Equilibrium Constant, a student combines equimolar amounts of acetic acid and ethanol to react as shown by the following equation. acetic acid + ethanol ethyl acetate + water To determine the initial concentration of acetic acid, 1.00mL of the resulting mixture was titrated with 0.2100MNaOH, requiring 33.25mL. What is the molarity of the acetic acid

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