3. A student uses a class B burette (the error on this burette is + 0.1 mL) to complete aredox titration with potassium permanganate added to a sample containing aqueousiron (the balanced reaction is below). An Erlenmeyer flask contains the iron solutionand the titrant is an aqueous solution of 0.125 M KMNO4. The initial volume of KMNO4in the burette is recorded as "five milliliters" with a final volume recorded as "twelvemilliliters." This is the volume it took to completely react all of the iron in the sample.5 Fe?* (aq) + MnO4" (aq) + 8 H* (aq) → Mn²* (aq) + 5 Fe* (aq) + 4 H2O (1)What is the absolute error on the calculated milligrams of iron in this sample?a. ± 10 mgb. ±3 mgc. 17 mgd. +0.7 mge. +4 mg

No of moles = Molarity * Volume (L) Mass = Moles * Molar mass

Answered: What is the absolute error on the…

What is the absolute error on the calculated milligrams of iron in this sample? a. ± 10 mg b. ±3 mg c. 17 mg d. +0.7 mg e. +4 mg

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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Question

3. A student uses a class B burette (the error on this burette is + 0.1 mL) to complete a
redox titration with potassium permanganate added to a sample containing aqueous
iron (the balanced reaction is below). An Erlenmeyer flask contains the iron solution
and the titrant is an aqueous solution of 0.125 M KMNO4. The initial volume of KMNO4
in the burette is recorded as "five milliliters" with a final volume recorded as "twelve
milliliters." This is the volume it took to completely react all of the iron in the sample.
5 Fe?* (aq) + MnO4" (aq) + 8 H* (aq) → Mn²* (aq) + 5 Fe* (aq) + 4 H2O (1)
What is the absolute error on the calculated milligrams of iron in this sample?
a. ± 10 mg
b. ±3 mg
c. 17 mg
d. +0.7 mg
e. +4 mg

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