Iron(II) sulfate, is typically the source of iron in tablets prescribed to anemic patients, a condition where a person lacks enough healthy red blood cells. The tablets can be dissolved in dilute sulfuric acid to dissolve the Fe2+ ions. To determine the percentage by mass of iron within the tablets, the Fe2+ ions can be oxidised to Fe3+ using potassium permanganate, where MnO4− is reduced to Mn2+. Calculate the percentage by mass of iron in a 500 mg tablet that requires 24.53 cm3 of 0.0100 mol dm−3 KMnO4 to titrate the iron sample. State your answer to 3 significant figures. M(Fe) = 55.85 g mol−1
Iron(II) sulfate, is typically the source of iron in tablets prescribed to anemic patients, a condition where a person lacks enough healthy red blood cells. The tablets can be dissolved in dilute sulfuric acid to dissolve the Fe2+ ions. To determine the percentage by mass of iron within the tablets, the Fe2+ ions can be oxidised to Fe3+ using potassium permanganate, where MnO4− is reduced to Mn2+. Calculate the percentage by mass of iron in a 500 mg tablet that requires 24.53 cm3 of 0.0100 mol dm−3 KMnO4 to titrate the iron sample. State your answer to 3 significant figures. M(Fe) = 55.85 g mol−1
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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Iron(II) sulfate, is typically the source of iron in tablets prescribed to anemic patients, a condition where a person lacks enough healthy red blood cells. The tablets can be dissolved in dilute sulfuric acid to dissolve the Fe2+ ions. To determine the percentage by mass of iron within the tablets, the Fe2+ ions can be oxidised to Fe3+ using potassium permanganate, where MnO4− is reduced to Mn2+.
Calculate the percentage by mass of iron in a 500 mg tablet that requires 24.53 cm3 of 0.0100 mol dm−3 KMnO4 to titrate the iron sample. State your answer to 3 significant figures.
M(Fe) = 55.85 g mol−1
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