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Ch.10 - Acid-Base TitrationsWorksheetSee all chapters

# Weak Acid-Strong Base Titrations

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Sections
Strong Acid-Strong Base Titrations
Weak Acid-Strong Base Titrations
Weak Base-Strong Acid Titrations
Diprotic Acid Titrations
Polyprotic Titrations
###### Weak Acid-Strong Base Titrations

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.

###### Weak Acid-Strong Base Titrations CalculationsĀ

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.