What is the rationale of maintaining the analyte solution at high pH (~10) in the titration process with EDTA? At this pH, EDTA is at its fully deprotonated form, Y-4. At this pH, EDTA is partially deprotonated with 1 ionizable H+. At this pH, EDTA is at its fully protonated form, H4Y. At this pH, EDTA is partially deprotonated with 2 ionizable H+.

What is the rationale of maintaining the analyte solution at high pH (~10) in the titration process with EDTA? At this pH, EDTA is at its fully deprotonated form, Y-4. At this pH, EDTA is partially deprotonated with 1 ionizable H+. At this pH, EDTA is at its fully protonated form, H4Y. At this pH, EDTA is partially deprotonated with 2 ionizable H+.

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 solution containing Mg2+ was buffered to pH 9.75 and titrated with EDTA. Eriochrome black T, with pKa1 = 6.3 and pKa2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator's most prevalent species at this pH) Review text sections 10.4 and 10.5 for help with this!
A solution containing Mg2+ was buffered to pH 9.81 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)
In a Complexometric Titration Experiment, the preparation of the EDTA solution is as follows: In a 250 mL beaker, weigh 0.10 g MgCl2*6H2O and 1.0 g NaOH. Add approximately 200 mL distilled water and stir to dissolve. Add about 2.0 g of EDTA and transfer the solution quantitatively to a 1-L volumetric flask. Dilute to the mark with distilled water. What is the purpose of adding MgCl2*6H2O? Please show COMPLETE solution.
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 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?
Calculate the molar solubility of calcium oxalate in a solution that has been buffered so that its pH is constant and equal to 4.00. Data: Kps of CaC2O4 = 1.7x10 -9 ; Ka1 of H2C2O4 = 5.60x10-2 and Ka2 = 5.42x10-5 . Use systematic treatment.
An aliquot of 20 ml of skim milk was placed in an Erlenmeyer flask. To the flask was added 3 to 4 drops of phenolphthalein. The sample was titrated in triplicate using a previously standardized NaOH solution 0.101M. The volumes of NaOH spent in the three experiments to reach chemical equivalence were 3.6ml, 3.7ml and 3.5ml. 1) Express the acidity of milk in g/L of lactic acid. 2) Assuming that the only acid present in milk is lactic acid, would you expect the pH corresponding to the equivalence point was 7?.
A 30-ml portion of a solution containing Ca²+ and Mg2+ was titrated with 28.19 mL of 0.207 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 0.054 M of Mg2+ in the sample? Express your answer with 2 decimal places and do not encode the units.
25.0 cm3 of sodium hydroxide solution is tritrated against 0.2 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.Phenolphthalein is used as an indicator in the above experiment. What will be its colour change at the end point? From pink to yellow From pink to colourless From yellow to colourless From yellow to pink
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.
(ii) Consider the titration of 25.00 mL of 0.02000 M CaSO4 with 0.01000 M EDTA at pH 10.00. Write the chemical equation for this titration and calculate the conditional formation constant for this reaction. (iii) From (ii) calculate the concentration of Ca2+ and pCa2+ at the volume of 20.0 mL of EDTA added.
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.

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		At this pH, EDTA is at its fully deprotonated form, Y^-4.
		At this pH, EDTA is partially deprotonated with 1 ionizable H⁺.
		At this pH, EDTA is at its fully protonated form, H₄Y.
		At this pH, EDTA is partially deprotonated with 2 ionizable H⁺.