Concept #1: In these series of titrations the weak acid is the starting solution or analyte and the strong base is the titrant.
Concept #2: Before the equivalence point has been reached we have the formation of a buffer and the Henderson Hasselbalch Equation can be utilized.
Concept #3: At the equivalence point we have no remaining weak acid or strong base, but instead an excess of conjugate base.
Concept #4: Beyond the equivalence point we will have an excess of strong base and conjugate base remaining.
Example #1: Consider the titration of 75.0 mL of 0.0300 M H3C3O3 (Ka = 4.1 X 10-3) with 30.0 mL of 0.0450 M KOH. Calculate the pH.
Example #2: Consider the titration of 50.0 mL of 0.150 M HF with 0.100 M NaOH at the equivalence point. What would be the pH of the solution at the equivalence point? The Ka of HF is 3.5 x 10-4.
