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

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.31QAP

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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?
A 25.00 mL sample containing Fe3+ was treated with 10.00 mL of 0.03676 M EDTA to complex all the Fe3+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 2.37 mL of 0.04615 M Mg2+. What was the concentration of Fe3+ in the original solution in ppm Fe3+?
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.
Assess the validity of each statement and choose X if the statement is CORRECT, Choose Y if otherwise. 10. Potentiometric methods can be used for end-point detection in EDTA titration of metal ions for which ion electrodes are available 11. Back titrations are useful for determining cations that are able to form stable EDTA complexes. 12. Nitriloacetic acid is an aminopolycarboxylic acid. 13. A ligand that has a single donor group is unidentate such as glycine. 14. Ammonia is a bidentate ligand. 15. The term chelate is derived from a Greek word meaning, toothlike projections
b. EDTA cannot be used as a primary standard always. When can EDTA be used as a primarystandard ? Give reason why EDTA is used in complexometric titrations.
A 25.00-mL sample containing Fe3+ was treated with 10.00 mL of 0.036 7 M EDTA to complex all the Fe3+ and leave excess EDTA in solution. The excess EDTA was then back titrated, requiring 2.37 mL of 0.0461 M Mg2+. What was the concentration of Fe3+ in the original solution?
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Calculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 26.0 mL
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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.
1. an accurately weighed chelometric standard calcium carbonate of 150 mg was used to standardize Disodium ethylenediaminetetraacetate, using the same procedure set by the monograph. The total volume of EDTA consumed was 37.5 ml . Calculate the molarity and normality of the standard solution. 2. A 0.62L of 0.072N silver nitrate was used to titrate three samples of sodium lauryl sulfate with 2500 mg,5000mg, and 6750 mg respectively. Tabulate its data, calculate the %NaCl in each sample , did any sample conformed to the official requirement?
Calculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 5.00 mL After the addition of 26.00 mL