EDTA is one of the common reagents used in a complexometric titration. a. Can we use EDTA titrations to determine the concentration of halides in a sample? Give reason for your answer. b. Why is EDTA used to determine concentration of a metal ion in a solution. c. Why is Erichrome black -T used as the indicator in EDTA titrations ?

EDTA is one of the common reagents used in a complexometric titration. a. Can we use EDTA titrations to determine the concentration of halides in a sample? Give reason for your answer. b. Why is EDTA used to determine concentration of a metal ion in a solution. c. Why is Erichrome black -T used as the indicator in EDTA titrations ?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter26: Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 26.12QAP

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Elaborate the reason why EDTA is used in many complexometric titrations. How will you be able to improve its selectivity when it comes to analyzing specific metals?
2. EDTA is one of the common reagents used in a complexometric titration. a. Can we use EDTA titrations to determine the concentration of halides in a sample? Give reason for your answer. b. Why is EDTA used to determine concentration of a metal ion ina solution. c. Why is Erichrome black -T used as the indicator in EDTA titrations ? d. Explain hardness of water. Why is it usually expressed in terms of Ca2+ ions?
Which of the following statements is TRUE about EDTA titration? A. Eriochrome black T is a titrant in EDTA titration B. EDTA titration can be used in the quantification of metals. C. EDTA titration is pH independent D. EDTA gives a sharper endpoint compared to a unidentate ligand. E. EDTA combines with metal in 1:6 ratio.
What is the purpose of adding concentrated ammonia in the elimination test for cations? Select one: a. because NH3 is a stronger base than NaOH b. to provide a strongly basic solution c. to determine if the hydroxide precipitates are amphoteric d. to determine if the test ions form NH3 complexes e. to determine if the NH3 solution oxidizes the test ions
In complexation volumetry, classify the statements below as true or false.Justify the one(s) that you judge to be “false”.a) When preparing an EDTA solution, to be used as a titrant of Ca2+ ions, it is necessary to add a small amount of Mg2+ in the solution.b) A metallochromic (Ind) indicator is a substance that forms colored complexes with metallic ions. The colors of these complexes are always the same as the colors of the free forms of these indicators.c) In order for the titration of a metal (Me) with EDTA to be carried out, it is necessary that the Me-EDTA complex has a stability constant greater than that of the Me-Ind complex.d) In determining the partial hardness of a hard water sample with EDTA solution, murexide is used as an indicator at pH 10.
Why is the solution containing the metal ion buffered before titrating with EDTA?
The Zn in a 0.7556-g sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. Calculate the percentage of Zn in this sample. A silver nitrate solution contains 14.77 g of primary-standard grade AgNO3 in 1.00 L. What volume of this solution will be needed to react with 0.2631 g of NaCl.
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. What is the structure and full name for EDTA? b. The titration of Zn^+2 and EDTA is carried out in the same manner as the Mg^+2 * EDTA titration (in fact, Zn metal may be used to standardize your EDTA solution). In this case, the ammonia from the pH 10 buffer serves an additional purpose. What is it? c. Although EDTA has, in its fully protonated form, 4 hydrogen atoms that can be lost, it is listed as a hexadentate ligand. Explain why this is the case.
Which is NOT true about EDTA? a. EDTA acts as a complexing agent in compleximetric titrations b. EDTA acts as a lewic acid in formation of complexes c. EDTA forms a 1:1, stable, water-soluble complex d. EDTA has high formation constants with metals.
what is the purpose of introducing ammonim sulphate to the mixture when determing the formula of a complex ion using colorimetric method
Complex Ion Formation and Precipitation Reactions i. A 1-L water sample was submitted for determination of chloride ion. 100.00mL the sample was analyzed using the Volhard method. 50.00 mL of 0.0929N AgNO3 was added to the sample and was back titrated with 12.50mL of 0.0510N KSCN solution to reach the end point. Find ppm Cl- in the water sample. ii. Using Mohr method, the chloride content of a mineral water was determined. 50.00mL of the sample was titrated with 10.80mL of 0.05N AgNO3 solution to reach end point. Determine the concentration of Cl- in ppm. iii. Calculate the hardness of a water sample such that 100.00mL of the sample required 35.00mL of 0.1051M EDTA solution to reach the end point.