A typical sample of iron ore contains both Fe2+ and Fet jons, The total amount of iron present in the ore can be determined by dissolving a sample of the ore in an acid solution, reducing all the iron present to Fe* and titrating the resulting solution with a standard potassium permanganate solution as follows: A 4.730 g sample of the ore is dissolved in hydrochloric acid and passed over a reducing agent to convert all the iron to Fe?+. • This solution is quantitatively transferred to a 150.00 mL volumetric flask and made up to the mark. • A 15.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.0512 M KMNO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns a bright pink due to the presence of excess permanganate ions. The average titration value is 31.60 mL of the KMNO, solution. The reaction stoichiometry is as follows: KMN0, (aq) + 8HCE(aq) + 5FeClz(aq) - 2MnCl2(aq) + 4H20 (8) + 5FeCcez (aq) + KCe (aq) 1.1 Determine the percentage of iron in the ore. Naturally occurring manganese consists of only the Mn isotope. Determine the moles of the manganese salt formed, and then calculate the total number of neutrons present in all the manganese 1.2 ions in the final solution.
A typical sample of iron ore contains both Fe2+ and Fet jons, The total amount of iron present in the ore can be determined by dissolving a sample of the ore in an acid solution, reducing all the iron present to Fe* and titrating the resulting solution with a standard potassium permanganate solution as follows: A 4.730 g sample of the ore is dissolved in hydrochloric acid and passed over a reducing agent to convert all the iron to Fe?+. • This solution is quantitatively transferred to a 150.00 mL volumetric flask and made up to the mark. • A 15.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.0512 M KMNO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns a bright pink due to the presence of excess permanganate ions. The average titration value is 31.60 mL of the KMNO, solution. The reaction stoichiometry is as follows: KMN0, (aq) + 8HCE(aq) + 5FeClz(aq) - 2MnCl2(aq) + 4H20 (8) + 5FeCcez (aq) + KCe (aq) 1.1 Determine the percentage of iron in the ore. Naturally occurring manganese consists of only the Mn isotope. Determine the moles of the manganese salt formed, and then calculate the total number of neutrons present in all the manganese 1.2 ions in the final solution.
Chemistry
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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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Solution Stoichiometry
1
A typical sample of iron ore contains both Fe2+ and Fe+ jons, The total amount of iron present in the
ore can be determined by dissolving a sample of the ore in an acid solution, reducing all the iron present
to Fe and titrating the resulting solution with a standard potassium permanganate solution as follows:
A 4.730 g sample of the ore is dissolved in hydrochloric acid and passed over a reducing agent to
convert all the iron to Fe2+.
• This solution is quantitatively transferred to a 150.00 mL volumetric flask and made up to the mark.
A 15.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.0512 M KMN04
solution.
• The endpoint of the titration is determined when the colourless solution in the conical flask turns a
bright pink due to the presence of excess permanganate ions.
• The average titration value is 31.60 mL of the KMNO4 solution.
The reaction stoichiometry is as follows:
KMN0,(aq) + 8HC{(aq) + 5FeC£z(aq) → 2MnC{2(aq) + 4H20 (f) + 5FEC{z (aq) + KC£ (aq)
1.1
Determine the percentage of iron in the ore.
Naturally occurring manganese consists of only the Mn isotope. Determine the moles of the
manganese salt formed, and then calculate the total number of neutrons present in all the manganese
1.2
ions in the final solution.
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