A scientist needed to determine the concentration of a solution of iron(II) ions. To do this, they titrated 40.0 mL of the analyte against 0.0100 M potassium permanganate solution. The titration was repeated multiple times to improve the accuracy. Determine the concentration of the solution of iron (II) ions.
A scientist needed to determine the concentration of a solution of iron(II) ions. To do this, they titrated 40.0 mL of the analyte against 0.0100 M potassium permanganate solution. The titration was repeated multiple times to improve the accuracy. Determine the concentration of the solution of iron (II) ions.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:A scientist needed to determine the concentration of a solution of iron(II) ions. To do this, they titrated 40.0 mL
of the analyte against 0.0100 M potassium permanganate solution. The titration was repeated multiple times to
improve the accuracy.
Determine the concentration of the solution of iron (II) ions.
a Choose the correct titration runs, and calculate the average titer
of potassium permanganate.
(To avoid introducing rounding errors on intermediate
calculations, enter your answer to five significant figures.)
Average titer of potassium permanganate =
ml
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Trial Run Titer
Run 1 Titer
Run 2 Titer
Run 3 Titer
Run 4 Titer
14.20 ml
13.30 mL
13.10 mL
11.60 mL
13.20 mL
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