A sample of an iron ore is dissolved in acid, and the iron isconverted to Fe2+. The sample is then titrated with 47.20 mLof 0.02240 M MnO4- solution. The oxidation-reduction reactionthat occurs during titration isMnO4-1aq2 + 5 Fe2+1aq2 + 8 H+1aq2¡Mn2+1aq2 + 5 Fe3+1aq2 + 4 H2O1l2(a) How many moles of MnO4- were added to the solution?(b) How many moles of Fe2+ were in the sample? (c) Howmany grams of iron were in the sample? (d) If the samplehad a mass of 0.8890 g, what is the percentage of iron in thesample?
A sample of an iron ore is dissolved in acid, and the iron isconverted to Fe2+. The sample is then titrated with 47.20 mLof 0.02240 M MnO4- solution. The oxidation-reduction reactionthat occurs during titration isMnO4-1aq2 + 5 Fe2+1aq2 + 8 H+1aq2¡Mn2+1aq2 + 5 Fe3+1aq2 + 4 H2O1l2(a) How many moles of MnO4- were added to the solution?(b) How many moles of Fe2+ were in the sample? (c) Howmany grams of iron were in the sample? (d) If the samplehad a mass of 0.8890 g, what is the percentage of iron in thesample?
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
A sample of an iron ore is dissolved in acid, and the iron is
converted to Fe2+. The sample is then titrated with 47.20 mL
of 0.02240 M MnO4
- solution. The oxidation-reduction reaction
that occurs during titration is
MnO4
-1aq2 + 5 Fe2+1aq2 + 8 H+1aq2¡
Mn2+1aq2 + 5 Fe3+1aq2 + 4 H2O1l2
(a) How many moles of MnO4
- were added to the solution?
(b) How many moles of Fe2+ were in the sample? (c) How
many grams of iron were in the sample? (d) If the sample
had a mass of 0.8890 g, what is the percentage of iron in the
sample?
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