What is the pH at the stoichiometric point?

Question

102. mL of a solution of quinine contains 206.0 x 10-3 mol of quinine. If this is titrated with 0.0200 M HCl, what is the pH at the stoichiometric point? Quinine is monobasic with
Kb = 7.90 x 10-6

any help would be greatly appreciated!

Answer 1

What do you mean about "stoichiometric point"? If that means half of the quinine converted to the conjugated acid form and half of quinine left in the basic form, the pH is:
pH = 14 + log(Kb) = 14 + log(7.90 x 10-6).
You do the math.