What is the value of [Mg2+] and pMg for 20.0 mL of a 0.020 M Mg2+ solution buffered at pH 10.00 and titrated with 0.020 M EDTA. K₁=6.2 x 108 and CY4- at pH 10.0= 0.30 a- when 5.0 mL of EDTA is added? b- when 20.0 mL of EDTA is added? c- when 25.0 mL of EDTA is added?
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- Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn at the equivalence point of the titration?Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn of the solution after 30 mL of titrant have been added?Determine the molar concentration of an EDTA solution of which 26.44 mL were required to titrate a sample containing 287.4 mg of primary standard CaCO3.
- 50.00 mL of a solution containing iron (II) and iron (III) when titrated at pH2.0, 12.50 mL 0.01200 M EDTA and when titrated at pH 6.0, 28.50 mL EDTA is spent. Find the concentration of each solute in this solution in ppm. (Fe (AA) = 55,847 g / mol) A. 184 ppm Fe3+, 213 ppm Fe2+B. 167,5 ppm Fe3+, 214,4 ppm Fe2+C. 213 ppm Fe3+, 184 ppm Fe2+D. 214,4 ppm Fe3+, 167,5 ppm Fe2+50.00 mL of 0.0524 M Pb(NO3)2 is titrated with 0.0419 M EDTA. The pH is buffered to 8.57. Find the following concentrations, [EDTA], [Y-4], [PbY-2] and [Pb+2], at each of the points described below. A. After 30.00 mL of EDTA has been added. B. At the endpoint. C. After 70.56 mL of EDTA has been added.In the titration of MgSO4.nH2O (2g per litre) against a 0.01 M solution of the disodium salt of ethylenediamine tetraacetic acid (EDTA) the titres obtained were as follows ; titre 1: start - 0.7 ml and end - 13.3 ml (12.6ml) titre 2: start - 13.3 ml and end 25.7 ml (12.4ml) Q. Calculate the value of n
- 50.00 mL of a solution containing iron (II) and iron (III) when titrated at pH2.0, 12.50 mL 0.01200 M EDTA and when titrated at pH 6.0, 28.50 mL EDTA is spent. Find the concentration of each solute in this solution in ppm. (Fe (AA) = 55,847 g / mol)The amount of calcium in physiologic fluids can be determined by a complexometric titration with EDTA. In one such analysis, a 0.100-mL sample of blood serum was made basic by adding 2 drops of NaOH and titrated with 0.00376 M EDTA, requiring 0.135 mL to reach the end point. Report the concentration of calcium in the sample as miligrams of Ca per 100 mL. (Ca = 40.078 amu).In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration? A. 0.040B. 0.044C. 0.021D. 0.027
- A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0474 M EDTA. The endpoint volume was 40.99 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0474 M EDTA and the endpoint volume was found to be 30.04 ml.Calamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?Given that the titration of Ca2+ and Mg2+ in a 50.00-mL sample of hard water required 22.35 mL of 0.01115 M EDTA. A second 50.00-mL aliquot was made strongly basic with NaOH to precipitate the Mg2+ as Mg(OH)2(s) . The supernatant liquid was titrated with 15.19 mL of the EDTA solution. Calculate the concentration in ppm of CaCO3 in the sample.