Solve the following problem related to the solubility equilibrium in an aqueous solution. The solubility of PbBr₂ is 0.384 gram per 100.0 mL of solution at 25°c.

1. Write the balanced chemical equation for the dissociation of PbBr₂ in aqueous solution.

2. Calculate the solubility (in moles per liter) of PbBr₂ at 25°c

3. Calculate the value of the solubility-product constant, Ksp for PbBr₂ at 25°c

Problems (4-6)

At 25°C Ksp for Ca(OH)_2(s) is 5.0 x 10^-6

4. Calculate the molar solubility of Ca(OH)₂ at 25C.

5. Calculate the molar solubility of Ca(OH)₂ at 25C in a pH 10.5 solution.

6. If 25.0mL of 0.00345M magnesium nitrate is mixed with 48.0 mL of 0.00056M sodium fluoride. Will a precipitate form. Given KSp magnesium fluoride = 6.4 x 10^-9

7. How many grams of solid NaOH must be added to 100.0mL of 0.25M HNO₂ to obtain a buffer solution that has a pH of 5.25? Assume the addition of the solid NaOH results in a negligible change in volume. Ka = 4.0 x10^-4

8. 25.0mL of barium hydroxide is titrated to the equivalence point with 36.5mL of 0.15M hydrochloric acid. What is the molarity of the barium hydroxide.