Ch.10 - Acid-Base TitrationsWorksheetSee all chapters
All Chapters
Ch.1 - Chemical Measurements
Ch.2 - Tools of the Trade
Ch.3 - Experimental Error
Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods
Ch.6 - Chemical Equilibrium
Ch.7 - Activity and the Systematic Treatment of Equilibrium
Ch.8 - Monoprotic Acid-Base Equilibria
Ch.9 - Polyprotic Acid-Base Equilibria
Ch.10 - Acid-Base Titrations
Ch.11 - EDTA Titrations
Ch.12 - Advanced Topics in Equilibrium
Ch.13 - Fundamentals of Electrochemistry
Ch.14 - Electrodes and Potentiometry
Ch.15 - Redox Titrations
Ch.16 - Electroanalytical Techniques
Ch.17 - Fundamentals of Spectrophotometry
BONUS: Chemical Kinetics
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 Calculations 

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.