1. ERT207 Analytical Chemistry Complexometric Titration
Pn Syazni Zainul Kamal
PPK Bioproses

2. CO4: ABILITY TO DIFFERENTIATE AND CALCULATE CONCENTRATION OF ANALYTES OF VARIOUS TITRIMETRIC METHODS (ACID-BASE, COMPLEXATION, REDOX, PRECIPITATION)

3. Types of Titrimetric Methods
Classified into four groups based on type of reaction involve;
Acid-base titrations
Complexometric titrations
Redox titrations
Precipitation titrations

4. Complexes
Most metal ions (kation) can react with lone pair electron from a molecule or anion to form covalent bonds and produce coordination compound or complexes.
Molecule or ion with at least 1 pair of unshared electron can form covalent bond with metal ion = ligands
The bonding between metal and ligand generally involves formal donation of one or more of the ligand's electron pairs
Eg of ligands = ammonia, cyanide ions, halide ions, water (neutral/-ve charge mols or ions)

5. Metal ion – lewis acid (electron pair acceptor)
Compound form between ligand and metal ion = complexes or coordination compound (has charges or neutral).
Examples of complex formation :
Ag CN Ag(CN)2-
Ag NH Ag (NH3)2+
Complex/coordination compound
Metal ion
ligand
Metal ion – lewis acid (electron pair acceptor)
Ligand – lewis base (electron pair donor)
Coordination number – number of covalent bond formed
between metal ion and ligand

6. A ligand that has one pair of unshared electron such as NH3, is called unidentate.
Glycine (NH2CH2COOH) and ethylenediamine (NH2CH2CH2NH2) which has two pairs of unshared electron available for covalent bonding, is called bidentate.
EDTA, has 6 pairs of unshared electrons = hexadentate

7. EDTA Equilibrium
Chelating agent - An organic agent that has two or more group capable of complexing with a metal ion (also called ligand)
Chelate – complex formed
Titration with chelating agent = chelometric titration , a type of complexometric titration
Most widely used chelating agent in titration – ethylenediaminetetraacetic acid (EDTA).

9. EDTA = Ethylenediaminetetraacetic acid
Hexadentate ligand
Has six bonding sites (the four carboxyl groups and the two nitrogen providing six lone pairs electrons)
Tetraprotic acid (H4Y), can exist in many forms H3Y-, H2Y2-, HY3- and Y4-
only unprotonated ligand (Y4-) can complex with metal ion

10. H4Y H+ + H3Y- Ka1 = [H+][H3Y-] = 1.0 x10-2
Since EDTA is a tetraprotic acid, the dissociation of EDTA as follows :
H4Y H+ + H3Y Ka1 = [H+][H3Y-] = 1.0 x10-2
[H4Y]
H3Y H+ + H2Y Ka2 = [H+][H2Y2-] = 2.1 x10-3
[H3Y-]
H2Y H+ + HY Ka3 = [H+][HY3-] = 6.9 x10-7
[H2Y2-]
HY H+ + Y Ka4 = [H+][Y4-] = 5.5 x10-11
[HY3-]

11. Complex formation constant of EDTA
EDTA can form complex with Ca2+ as the following equilibrium :
Ca Y CaY (1)
The complex formation constant is :
Kf = KCaY2- = [CaY2-] (2)
[Ca2+][Y4-]

13. Effect of pH on EDTA equilibria
If H+ concentration increases, equilibrium in equation 1 will shift to the left.
Chelating anion (Y4-) will react with H+. Dissociation of CaY2- in presence of acid
From the overall equilibrium

14. Let us consider that CH4Y represent the total uncomplexed EDTA
If we substitute the values of [HY3-], [H2Y2-], [H3Y-] and [H4Y] derived from the Ka values to this equation and divide each term with [Y4-], we will get the following equation:-
Where α4 is the fraction of the total EDTA exists as Y4- .

15. Conditional formation constant
The equation for the complex formation between Ca and EDTA is :
Ca2+ + Y CaY (3)
Kf = KCaY2- = [CaY2-] (4)
[Ca2+][Y4-]
α4 = [Y4-] , hence [Y4-] = α4 CH4Y (5)
CH4Y

16. Replacing [Y4-] into equation (4) : Kf = KCaY2- = [CaY2-] (6)
[Ca2+] α4CH4Y
Kfα4 = [CaY2-] = K’f (7)
[Ca2+]CH4Y
K’f is the conditional formation constant which depends on α4
therefore K’f depends on pH. We can use equation (7) to calculate the value of equilibirum concentration for EDTA species at specific pH to replace equation (4)

17. Metal-EDTA titration curves
Titration is perform by adding the chelating agent (EDTA) to the sample (metal).
Titration curve – plotting the changes in metal ion concentration (pM) versus volume of titrant (EDTA)
Example of complexometric titration is by adding M EDTA to 100 ml M Ca2+ solution buffered at pH 11
Ca Y CaY2-

18. Before titration started – only have Ca2+ solution.
pCa = - log [Ca2+]
Titration proceed – part of Ca2+ is reacted with EDTA to form chelate. [Ca2+] gradually decrease.
pCa= -log [remaining Ca2+]
At equivalence point – have convert all Ca2+ to CaY2- So pCa can be determined from the dissociation of chelate at a given pH using Kf.
K’f = Kf α4 = [CaY2-]
[Ca2+] CH4Y
Excess titrant added – pCa can be determined from the dissociation of chelate at a given pH using Kf.

20. Exercise
Calculate pCa in 100 ml of a solution of M Ca2+ at pH10 after addition of 0, 50, 100, 150 ml of M EDTA. Kf for CaY2- is 5.0x1010 and α4 is 0.35.
K’f = Kf x α4
= 5.0x1010 x 0.35
= 1.75x1010

21. a) Addition of 0.00 ml EDTA
[Ca2+] = M
pCa = - log 0.100
= 1.00

22. b) Addition of ml EDTA
Initial mmol Ca2+ =100ml x M =10 mmol
mmol EDTA added = 50ml x M = 5 mmol
mmol Ca2+ left = 5 mmol
[Ca2+] = 5 mmol = M
(100+50)ml
pCa = - log = 1.48

23. c) Addition of 100 ml EDTA Initial mmol Ca2+ =100ml x 0.100 M =10 mmol
mmol EDTA added =100ml x M = 10 mmol
Equivalence point is reached. We have convert all Ca2+ to CaY2-. mmol CaY2- = mmol initial Ca2+
[CaY2-] = mmol = 0.05 M
( )ml
K’f = Kf α4 = [CaY2-]
[Ca2+] CH4Y
K’f = [CaY2-] = 1.75 x 1010
= 1.75 x 1010
(x)(x)
x = 1.7 x so pCa = - log 1.7x10-6 = 5.77

24. d) Addition of 150 ml EDTA Initial mmol Ca2+ =100ml x 0.100 M =10 mmol
mmol EDTA added =150ml x M =15 mmol
mmol EDTA excess = 5 mmol
CH4Y = 5 mmol = 0.02M [CaY2-] = = 0.04M
( )ml ( )ml
K’f = [CaY2-] = 1.75 x 1010
[Ca2+] (0.02)
= 1.75 x 1010
(x)(0.02)
x = 1.14 x so pCa = - log 1.14x10-10 = 9.94