A 13.00 g sample of an ionic compound NaA, where A- is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 550.0 mL of HCl was added, the pH was 5.00. The experimenter found that 1.10 L of 0.100 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.