During a titration of a weak base with a strong acid, you are slowing converting molecules of the weak base into molecules of its conjugate acid. For the hypothetical weak base, B we see the following: B (aq) + H3O+ (aq) â BH+ (aq) + H2O (l) In the problem below you will be adding some strong acid, but not enough to reach the endpoint of the titration. 1.80 mL of hydrochloric acid added to the weak base 2.00M hydrochloric acid in the buret as the titrant 11.0 mL of original 1.05 M NH3 (ammonia) sample You are titrating 11.00 mL of a 1.05 M solution of NH3 (ammonia) with a strong acid. If you add 1.80 mL of a 2.00 M solution of hydrochloric acid, what is the final pH of the remaining weak base solution? The kb for NH3 (ammonia) is 1.76 X 105. final pH =