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Ch.11 - EDTA 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
Metal Chelate Complexes
EDTA Titration Curves
EDTA Titrations

Concept #1: In these types of titration the ligand will serve as the titrant. 

Concept #2: Before the equivalence point is reached we have an excess of the metal ion remaining. 

Concept #3: At the equivalence point there are equal moles of the metal ion and the EDTA ligand. 

Concept #4: Beyond the equivalence point there is an excess of the EDTA ligand remaining. 

EDTA Titration Calculations 

Example #1: Calculate the pMn3+ for the titration of 30.0 mL of 0.0100 M EDTA with 50.0 mL of 0.0200 M MnPO4 at pH = 10.00.  

Practice: Calculate the pNi2+ for the titration of 50.0 mL of 0.120 M EDTA with 15.0 mL of 0.100 M NiCl­2 at pH = 8.22.