Question 3: Solubility Product Constant (35points) A. Silver bromide (AgBr) has a solubility of 7.07 × 10–7 mol/L. i. Write the dissolution reaction of AgBr, including all states. (0.5 points) ii. Write the expression for Ksp for AgBr. (0.5 points) iii. Calculate the solubility product constant of AgBr. (0.5 points) B. Lead(II) iodide (PbI2) has a solubility of 1.52 × 10–3 mol/L. i. Write the dissolution reaction of PbI2, including all states. (0.5 points) ii. Write the expression for Ksp for PbI2. (0.5 points) iii. What is the concentration of Pb2 in the equilibrium solution? (0.5 points) iv. What is the concentration of I– in the equilibrium solution? (0.5 points) v. Calculate the solubility product constant of PbI2. (0.5 points) C. PbSO4 has a Ksp = 1.3 × 10–8 (mol/L)2. i. Write the dissolution reaction of PbSO4, including all states. (0.5 points) ii. Write the expression for Ksp for PbSO4. (0.5 points) iii. Calculate the solubility of PbSO4. (0.5 points) D. Barium fluoride (BaF2) has a Ksp = 2.5 × 10–5 (mol/L)3. i. Write the dissolution reaction of BaF2, including all states. (0.5 points) ii. Write the expression for Ksp for BaF2. (0.5 points) iii. Write the Ksp expression as an algebraic equation, using the variable x to represent concentrations. (1 point) iv. Find the solubility of BaF2 by solving the equation you wrote in part iii. (0.5 points)