Consider a titration of 43.8mL of .124 M solution of aqueous ammonia [Kb(NH3)=1.8*10-5] with a .124 M solution of hydrochloric acid. Compute
A: The pH of the aqueous ammonia solution before titration
B: The pH of the solution at half equivalence point.
C: The pH of the solution at the equivalence point
D: The pH of the solution when 1.00mL of the HCl have been added after the equivalence point was reached.