• EDTA Titrations

• Chelation in Biochemistry

• Metal-Chelate Complexes

• Metals are Lewis acids that accept electron pairs from donating ligands that act as Lewis bases

–CN- is a common monodentate ligand, binding to a metal ion through one atom (C)

–Metals can bind to multiple ligands (usually 6)

• A ligand that can attach to a metal by more than one atom is multidentate or a chelating ligand

• Chelating agents can be used for titration of metals to form complex ions (complexometric titration)

• Chelating Agents in Analytical Chemistry

• Ethylenediamenetetraacetic acid (EDTA)

• Acid/Base Properties of EDTA

• EDTA is a hexaprotic system (H6Y2+) with 4 carboxylic acids and 2 ammoniums:

• We usually express the equilibrium for the formation of complex ion in terms of the Y4- form (all six protons dissociated). You should not take this to mean that only the Y4- form reacts

• Fraction of EDTA in Y4- Form

• Similar to acids and bases, we can define fractional compositions, α, defined as the fraction of “free” EDTA in a particular form.

–“Free” means uncomplexed EDTA

–So, for Y4-:

• EDTA Complexes

• The equilibrium constant for a reaction of metal with EDTA is called the formation constant, Kf, or the stability constant:

• Again, Kf could have been defined for any form of EDTA, it should not be understood that only the Y4- reacts to form complex ion.

• pH Dependence of αY4-

• Formation Constants for M-EDTA Complexes

• Some Metals Form 7 or 8 Coordinate Complexes

• Conditional Formation Constant

• We saw from the fraction plot that most of the EDTA is not in the form of Y4- below a pH ~10.

• We can derive a more useful equilibrium equation by rearranging the fraction relationship:

• If we fix the pH of the titration with a buffer, then αY4- is a constant that can be combined with Kf

• Example

• Calculate the concentration of free Ca2+ in a solution of 0.10 M CaY2- at pH 10 and pH 6. Kf for CaY2- is 4.9×1010 (Table 13-2)

• At low pH, the metal-complex is less stable

• Calcium/EDTA Titration Curve

• Generic Titration Curve

• Before the Equivalence Point

• What’s pCa2+ when we have added 5.0 mL of EDTA?

• At the Equivalence Point

• What’s pCa2+ when we have added 25.0 mL of EDTA?

–At the equivalence point almost all the metal is in the form CaY2-

–Free Calcium is small and can be found w/ algebra

• After the Equivalence Point

• What’s pCa2+ when we have added 26.0 mL of EDTA?

–We have 1.0 mL excess EDTA

• Auxiliary Complexing Agents

• In aqueous solution, metal-hydroxide complexes or precipitates can form, especially at alkaline pH

• We often have to use an auxiliary complexing agent

–This is a ligand that binds strongly enough to the metal to prevent hydroxide precipitation, but weak enough to be displaced by EDTA

• Ammonia is a common auxiliary complex for transition metals like zinc

• Metal Ion Indicators

• To detect the end point of EDTA titrations, we usually use a metal ion indicator or an ion-selective electrode (Ch. 15)

• Metal ion indicators change color when the metal ion is bound to EDTA:

–Eriochrome black T is an organic ion

• The indicator must bind less strongly than EDTA

• Metal Ion Indicator Compounds

• EDTA Titration Techniques

• Direct titration: analyte is titrated with standard EDTA with solution buffered at a pH where Kf’ is large

• Back titration: known excess of EDTA is added to analyte. Excess EDTA is titrated with 2nd metal ion.

• EDTA Titration Techniques (2)

• Displacement titration: For metals without a good indicator ion, the analyte can be treated with excess Mg(EDTA)2-. The analyte displaces Mg, and than Mg can be titrated with standard EDTA

• Indirect titration: Anions can be analyzed by precipitation with excess metal ion and then titration of the metal in the dissolved precipitate with EDTA.

• Example Titration

• 25.0 mL of an unknown Ni2+ solution was treated with 25.00 mL of 0.05283 M Na2EDTA. The pH of the solution was buffered to 5.5 and than back-titrated with 17.61 mL of 0.02299 M Zn2+. What was the unknown Ni2+ M?

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