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Q: EDTA
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Why is EDTA complex formation less complete at lower pH?
Ethylenediamine tetraacetic acid (EDTA) is a polyprotic acid containing four carboxylic acid groups and two amine groups with lone-pair electrons that chelate calcium and several other metal ions
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- Ethylenediaminetetraacetate (EDTA4 ) is used as a complexing agent in chemical analysis with the structure shown in Fig. 21.7. Solutions of EDTA4 are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The complex ion virtually prevents the heavy metal ions from reacting with biochemical systems. The reaction of EDTA4 with Pb2+ is Pb2+(aq) + EDTA4(aq) iPbEDTA2(aq) K = 1.1 1018 Consider a solution with 0.010 mol of Pb(NO3)? added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na1EDTA. Does Pb(OH)2 precipitate from this solution? [Ksp for Pb(OH)2 = 1.2 1015.In which part of the oxalate ion acts as bidentate in complex formation reactions? K2Cr207 + 7H2C204 · 2H2O 2K[Cr(C204)2(H2O)2] · 2H2O + 6CO2 + 13H20Cysteine is an amino acid with S as the donor atom. It forms complexes with Fe2*, Hg2+, Mg2+, and Zn2+. Which set of pKf assignments is CORRECT for the formation of complexes of these metals with cysteine? Fe-complex Hg-complex Mg-complex Zn-complex Set A pKf = 6.2 pKf = 14.4 pKf = <4 pKf = 9.8 Set B pKf = 14.4 pKf = <4 pKf = 6.2 pKf = 9.8 Set C pKf = 6.2 pKf = 9.8 pKf = <4 pKf = 14.4 Set D pKf = 6.2 pKf = <4 pKf =14.4 pKf = 9.8 A. Set A B. Set B C. Set C D. Set D
- The complex formation reaction is given by: Ca^2+ + EDTA = CaY^2- 1.Calculate the concentration of free Ca^2+ in a solution of 0.10M CaY^2- at pH 10.00,given that the formation constant for CaY^2- is 10^10.65 and aY4- =0.30 at a pH of 10.00 2.How would the amount of Ca^2+ in the solution change if the pH of the solution was lowered to the pH of 6.(Note:it is not necessary to do the calculation)Cadmium is an interferant because it forms a precipitate with o-phenanthroline. What effect would the formation of a Cd-o-phenanthroline precipitate have on thedetermination of the parts per million of Fe in a sample?When Fe2+ binds with EDTA why is the complex have a -2 charge
- What effect would it have on calculated value of Ksp if insufficient time was allowed for the Ca(IO3)2 solution to reach equilibrium?A spectrophotometric method for the determination of Fe (II) is based on the measurement of the red-orange color of its complex with o-phenanthroline. The complex obeys Beer's law for Fe (II) concentrations lower than 9 ppm. It is known that a solution containing 0.100 ppm of Fe(II) in excess of o-phenanthroline produces an absorbance of 0.200 in a cuvette with 1.00 cm of optical path and that an unknown sample gives an absorbance of 0.470 under the same conditions, Calculate: a) The concentration of Fe in the unknown sample in moles/L and ppm. b) The molar absorptivity coefficient of the complex. Fact. Fe = 55.845Calculate the Ksp for the slightly soluble salt Ce(IO3)4, if at equlibrium, the salt has measured concentration shown: [Ce4+] = 1.8 x 10-4 M [IO3-] = 2.6 x 10-13 M
- 1.Solution of EDTA is particularly valuable as titrants because the reagent combines with metal ions in a 1:1 ratio regardless of the charge on the cation. For example, Fe(ll) and Fe(ll), complexes are formed with EDTA with great stability. The formation constants for the Fe(ll)-EDTA chelate, and Fe(lll)-EDTA chelate are 2.1 x 1014 and 1.3 X 1025, respectively. a) For each ion complex mentioned above, write the equations of reactions for complex formation and expression for the complex formation constant. b) Calculate the concentration of Fet In a solution that was prepared by mixing 50.0 mL of 0.200 M Fohwith 200 0 o/oro.0100 M EDTA. The mixture was buffered to a ph of 11.00, (Given the valio of a, 0.85 al pH I1.00)iin the oxygen evolving centre in photosystem II the ground state electronic configuration of the proposed manganyl(V) complex isWhat is the LFSE for the [NiCl4]Cl2 complex?
