1. A student dissolves 0.01 mol of an unknown weak base in 100 ml water and titrates the solution with 0.1 M HNO3. After 40 ml of 0.1 M HNO3 was added, the pH of the resulting solution was 8.0. Calculate the Kb value for the weak base.

2. A 10 gram sample of the ionic compound NaA, where A is the anion of a weak acid was dissolved in enough water to make 100 ml of solution and was then titrated with 0.1 M HCL. After 500 ml HCL was added, the pH was 5. The experimenter found that 1 L of 0.1 M HCL was required to reach the stoichiometric point of the titration

A) what is the molar mass of NaA?
B) Calculate the pH of the solution at the stoichiometric point of the titration.

3. The concentratioin of Ag in a solution saturated with Ag2C2O4(s) is 2.2*10^-4M. Calculate the Ksp for Ag2C2O4.