Consider the following titration curve of a weak base titrated with a strong acid. How would the pH be calculated at point 1 on the curve? 14 12 2. 10 3 10 20 30 40 30 60 HCl added (mL) O By subtracting the mol of weak base initially present from the mol of strong acid added to calculate the molarity of strong acid O As a weak acid equilibrium using the K, and the concentration of acid added O As a weak base equilibrium using the Ki, and the concentration of base initially present As a buffer using using the K, and the ratio of weak base to conjugate acid Hd

In the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaOH a) the initial pH; b) pH after 50.0% completion of neutralization; c) pH after 100.0% completion of neutralization; d) Calculate the pH when 1 mL more NaOH is added after the equivalence point.

Calcuate the pH after 10ml of 1M HCL is added to the buffer if it was a 1L solution.

Determine the pH during the titration of 11.4 mL of 0.231 M nitric acid by 4.23x10-² barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 15.6 mL of barium hydroxide (3) At the equivalence point (4) After adding 39.2 mL of barium hydroxide 4