A sample of an ionic compound NaA, where A- is the anion of aweak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with0.100 M HCl. After 500.0 mL of HCl was added, the pH was measured and found to be 5.00. The experimenter found that 1.00 L of 0.100 M HClwas required to reach the stochiometric point of thetitration.
a. What is the Kb value for A-?
b Calculate the pH of the solution at the stochiometric point of the titration.