Given the approximate Kf values: Ca-EDTA = 1010 ; Mg-EDTA = 10 ; Fe-EDTA = 1014 ; Hg-EDTA = 1021; Zn-EDTA = 1016 Identify the correct statements. Mg2+ can be accurately analyzed by employing a back titration technique by titrating the excess EDTA with std Fe2+ solution. Hg2+ can be accurately analyzed by employing a back titration technique by titrating the excess EDTA with std Zn2+ solution. O Mg2+ cannot be directly titrated with EDTA using EBT indicator Fe2+ can be accurately analyzed by employing a back titration technique by titrating the excess EDTA with std Ca2+ solution

Given the approximate Kf values: Ca-EDTA = 1010 ; Mg-EDTA = 10 ; Fe-EDTA = 1014 ; Hg-EDTA = 1021; Zn-EDTA = 1016 Identify the correct statements. Mg2+ can be accurately analyzed by employing a back titration technique by titrating the excess EDTA with std Fe2+ solution. Hg2+ can be accurately analyzed by employing a back titration technique by titrating the excess EDTA with std Zn2+ solution. O Mg2+ cannot be directly titrated with EDTA using EBT indicator Fe2+ can be accurately analyzed by employing a back titration technique by titrating the excess EDTA with std Ca2+ solution

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

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A 50.0ml sample of water containing both Ca+2 and Mg+2 is titrated with 16.54ml of 0.01104M EDTA in an ammonia buffer of pH 10. Another 50.0ml sample is treated with NaOH to precipitate the Mg(OH)2 and then titrated at pH 13 with 9.26ml of the same EDTA solution. Calculate the ppm each of CaCO3 and MgCO3 in the sample.
A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508 nm after the addition of 1,10-phenanthroline, pH 4 buffer, and hydroxylamine. Then, a water sample treated similarly exhibited an absorbance of 0.109 au. Which of the following statements is true? (A) The Fe concentration of the water sample is higher than 100 ppm. B) The Fe concentration of the water sample is equal to 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. D) The Fe concentration of the water sample is lower than 100 ppm.
Average [EDTA] = C: Determination of the hardness of an unknown water sample: Using an unknown water sample, three 25 mL samples in 3 separate 250 mL Erlenmeyer flasks are prepared. To each flask, 5 mL of pH pH10 buffer, 3 to 5 drops of Eriochrome Black T indicator, and 15 drops of 0.03 M MgCl2 solution are added. Each flask is titrated to the end point using EDTA.
A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0421 M EDTA. The endpoint volume was 44.10 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 0.0421 M EDTA and the endpoint volume was found to be 35.11 ml.
A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0418 M EDTA. The endpoint volume was 44.36 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 0.0418 M EDTA and the endpoint volume was found to be 30.02 ml. Calculate the molar concentration of Mg.
A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508 nm after the addition of 1,10-phenanthroline, pH 4 buffer, and hydroxylamine. Then, a water sample treated similarly exhibited an absorbance of 0.109 au. Which of the following statements is true? The Fe concentration of the water sample is higher than 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. The Fe concentration of the water sample is lower than 100 ppm. The Fe concentration of the water sample is equal to 100 ppm.
A 0.4071-g sample of pure CaCO3 was transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. After transferring a 50.00-mL portion of this solution to a 250-mL Erlenmeyer flask, the pH was adjusted by adding 5 mL of a pH 10 buffer. After adding an indicator, the solution was titrated with the EDTA, requiring 42.63 mL to reach the end point. What is the concentration of EDTA? Choices: 0.0191 M, 0.0955 M, 0.00955 M, 0.477 M
Given the following problem: Na2CO3 + HCl -> NaCl + NaHCO3 Na2CO3 served as the primary standard in a titration experiment. 0.1g of the primary standard is weighed to the nearest 0.1 mg, and 75.0 mL boiled distilled water is added to dissolve the solid. It is then titrated with 0.1 M HCl solution until phenolphtalein endpoint. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
A 25.00 ml of Ni2* solution was diluted in HCI and treated with 25.00 ml of 0.05283 M NazEDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator. Back titration using standard 0.022 MZn2* at pH 5.5 requires 17.61 ml until end point, on which the solution will turn red. Calculate for the molarity of the unknown. Ans. 0.03664 M
A 30-mL portion of a solution containing Ca2+ and Mg2+ was titrated with 28.19 mL of 0.213 M EDTA at pH 10. Another 30-mL aliquot of the same Ca-Mg mixture was treated with NaOH to make the solution strongly alkaline and precipitate Mg(OH)2. This solution was then titrated with the same EDTA solution. What would be the required EDTA volume (in mL) to reach the endpoint of the second aliquot if it was found that there was 0.061 M of Mg2+ in the sample?
Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. A 50.00-mL sample of water containing Ca2+ and Mg2+ is titrated with 10.28 mL of 0.01001 M EDTA in an ammonia buffer at pH 10.00. Another 50.00-mL sample is titrated with NaOH to precipitate Mg(OH)2 and then titrated at pH 13.00 with 6.75 mL of the same EDTA solution. Calculate the concentration of CaCO3 and MgCO3 in the sample in ppm.