A solution of ammonia (0.12 M, 15.00 mL) was titrated with 0.2 M hydrochloric acid (K_b of ammonia = 1.8 $\times$ 10^-5). What is the pH at the equivalence point?

Question

Quizplus · Accepted Answer

At the equivalence point, the solution contains the ammonium ion (NH4+), which is the conjugate acid of ammonia. The pH is determined by the hydrolysis of NH4+, and using the Kb of ammonia, we can find the Ka of NH4+ and calculate the pH.

A Solution of Ammonia (0 ×\times× 10-5)

A Solution of Ammonia (0 $\times$ 10^-5)