A 0.200 -g sample of a triprotic acid (molar mass \(=165.0\) \(\mathrm{g} / \mathrm{mol}\) ) is dissolved in a \(50.00-\mathrm{mL}\) aqueous solution and titrated with \(0.0500 \mathrm{M} \mathrm{NaOH}\). After \(10.50 \mathrm{~mL}\) of the base was added, the \(\mathrm{pH}\) was observed to be 3.73. The \(\mathrm{pH}\) at the first stoichiometric point was 5.19 and at the second stoichiometric point was 8.00 .

a. Calculate the three \(K_{\mathrm{a}}\) values for the acid.

b. Make a reasonable estimate of the \(\mathrm{pH}\) after \(59.0 \mathrm{~mL}\) of \(0.0500 \mathrm{M} \mathrm{NaOH}\) has been added. Explain your answer.

c. Calculate the pH after \(59.0 \mathrm{~mL}\) of \(0.0500 \mathrm{M} \mathrm{NaOH}\) has been added.