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 Base-Strong Acid Titrations

Concept #1: In these series of titrations the weak base is the starting solution or analyte and the strong acid is the titrant.

Concept #2: Before the equivalence point has been reached we have the formation of a buffer and utilize the Henderson Hasselbalch Equation.

Concept #3: At the equivalence point we have no remaining weak base or strong acid, but instead an excess of conjugate acid or weak acid. 

Concept #4: Beyond the equivalence point we will have an excess of strong acid and conjugate acid or weak acid remaining. 

Weak Base-Strong Acid Titrations Calculations

Example #1: Consider the titration of 50.0 mL of 0.150 M CH3NH2 (Kb = 4.4 X 10-4) with 75.0 mL of 0.200 M HCl. Calculate the pH.

Example #2: Calculate the pH of the solution resulting from the mixing of 75.0 mL of 0.100 M NaC2H3O2 and 75.0 mL of 0.150 M HC2H3O2 with 0.0040 moles of HClO4. The Ka value of acetic acid is 1.8 x 10-5.