Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02156 M Fe²+ by 0.03517 M EDTA at a pH of 6.00. Thevalues for log Kf and ay can be found in the chempendix.13.00 mLpFe²+19.50 mL=the equivalence point, VepFe²+ =1.58IncorrectpFe2+ =10.31Incorrect6.376Incorrect

The question is based on the complexometric titration of ferrous ions and EDTA.We have to calculate…

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Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02156 M Fe²+ by 0.03517 M EDTA at a pH of 6.00. Th values for log Kf and ay can be found in the chempendix.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.54QE

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Question

Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02156 M Fe²+ by 0.03517 M EDTA at a pH of 6.00. The
values for log Kf and ay can be found in the chempendix.
13.00 mL
pFe²+
19.50 mL
=
the equivalence point, Ve
pFe²+ =
1.58
Incorrect
pFe2+ =
10.31
Incorrect
6.376
Incorrect

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Step 1: introduction

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Step 2: Ve and conditional formation constant determination

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Step 3: PFe2+ determination when volume of Fe2+ solution is 13 ml

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Step 4: PFe2+ determination at equivalence point

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Step 5: PFe2+ determination at equivalence point

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Step 6: determination of concentration of Y4- and FeY2- when volume of Fe2+ solution is 17.50 ml

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