Tutorial EDTA
Tutorial - EDTA and Complexmetric Titrations
FST 1113 Chemistry I
B.Sc. in Food Science & Nutrition and B.Sc. in Food Production & Technology Management
Department of Food Science and Technology, Faculty of Livestock, Fisheries and Nutrition
Semester 1- Academic Year 2013/2014
If you need additional data for this tutorial, please refer to literature 1. Define the following terms;
Chelate, ligand, coordination number, conditional formation constant.
2. Describe three general methods for performing EDTA titrations. What are the advantages of each?
3. With a suitable example explain how stepwise and overall formation constants are realated.
4. An EDTA solution was prepared by dissolving 3.853 g of purified and dried Na2H2Y.H2O in sufficient water to give 1.000 L. Calculate the molar concentration, given that the solute contained 0.3% excess moisture.
5. Calculate the weight of Na2H2Y.H2O required to prepare 500.00 mL of 0.0500 M EDTA.
6. A divalent metal ion M2+ reacts with a unidentate ligand (L) to form a 1:1 complex ML22+. Calculate the concentration of M2+ in a solution prepared by mixing equal volumes of 0.20 M M2+ and 0.20 M L if the Kf is 1.0 x 108.
7. Calculate the fraction of EDTA that exists as Y4- at pH 10, and from this calculate pCa in 100 mL of solution of 0.100 M Ca2+ at pH 10 after adding 100 mL of 0.100 M EDTA.
8. Silver ion forms a stable 1:1 complex with triethylenetetraamine {[“rien”, NH2(CH2)2NH(CH2)2NH(CH2)2NH2]. Calculate the silver ion concentration at equilibrium when 25 mL of 0.010 M silver nitrate is added to 50 mL 0f 0.015 M trien. Kf is 5.0 x 107.
9. Calculate the conditional constants for the formation of EDTA complex with Fe2+ at a pH of (a) 6.0 and (b) 8.0.
10. Calculate α4 and the mole percent of Y4- in a solution of EDTA that is buffered to (a) pH 3 and (b) 10.2. 11. Calculate the equilibrium concentration of Ni2+ in a solution prepared by dissolving 0.015 mol of NiY2- in 1 L of distilled water at pH (a) 3.0
FST 1113 Chemistry I
B.Sc. in Food Science & Nutrition and B.Sc. in Food Production & Technology Management
Department of Food Science and Technology, Faculty of Livestock, Fisheries and Nutrition
Semester 1- Academic Year 2013/2014
If you need additional data for this tutorial, please refer to literature 1. Define the following terms;
Chelate, ligand, coordination number, conditional formation constant.
2. Describe three general methods for performing EDTA titrations. What are the advantages of each?
3. With a suitable example explain how stepwise and overall formation constants are realated.
4. An EDTA solution was prepared by dissolving 3.853 g of purified and dried Na2H2Y.H2O in sufficient water to give 1.000 L. Calculate the molar concentration, given that the solute contained 0.3% excess moisture.
5. Calculate the weight of Na2H2Y.H2O required to prepare 500.00 mL of 0.0500 M EDTA.
6. A divalent metal ion M2+ reacts with a unidentate ligand (L) to form a 1:1 complex ML22+. Calculate the concentration of M2+ in a solution prepared by mixing equal volumes of 0.20 M M2+ and 0.20 M L if the Kf is 1.0 x 108.
7. Calculate the fraction of EDTA that exists as Y4- at pH 10, and from this calculate pCa in 100 mL of solution of 0.100 M Ca2+ at pH 10 after adding 100 mL of 0.100 M EDTA.
8. Silver ion forms a stable 1:1 complex with triethylenetetraamine {[“rien”, NH2(CH2)2NH(CH2)2NH(CH2)2NH2]. Calculate the silver ion concentration at equilibrium when 25 mL of 0.010 M silver nitrate is added to 50 mL 0f 0.015 M trien. Kf is 5.0 x 107.
9. Calculate the conditional constants for the formation of EDTA complex with Fe2+ at a pH of (a) 6.0 and (b) 8.0.
10. Calculate α4 and the mole percent of Y4- in a solution of EDTA that is buffered to (a) pH 3 and (b) 10.2. 11. Calculate the equilibrium concentration of Ni2+ in a solution prepared by dissolving 0.015 mol of NiY2- in 1 L of distilled water at pH (a) 3.0