A = NH₃, it has yet to be acidified.
B = NH₃ and NH₄ ⁺ in the buffering region.
C = NH₄ ⁺. At the equivalence point, all the NH₃ has been protonated, and water molecules begin to take up acidic protons.
D = NH₄ ⁺ and more acid in solution (H₃O⁺).

As we can see in the following titration curve, even if the pK _a of the indicator is several units away from the pH at the equivalence point, there is only a negligible change in volume of titrant added due to the steep slope of the titration curve near the equivalence point.

This is a standard stoichiometry problem for titration. Calculate the number of moles of base to know the number of moles of the unknown because it is a monoprotic acid. Once you know the number of moles of the unknown, divide the mass of the unknown by the number of moles to obtain the solution: the molecular weight of the unknown is 189.1 g/mol. Titration stoichiometry problems do not get much trickier than this.