The iron content of iron ore can be determined by titration with a standard KMNO4 solution. The iron ore is dissolved in HCl, and all the iron isreduced to Fe+ ions. This solution is then titrated with KMNO4 solution, producing Fe* and Mn2+ ions in acidic solution. If it required 42.41 mL of0.0452 M KMNO4 to titrate a solution made from 1.236 g of iron ore, what is the mass percent of iron in the iron ore?Mass percent =%

Answered: Image /qna-images/answer/9c6aab7d-6087-4dbb-b792-63e7e003084f.jpg

The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe+ ions. This solution is then titrated with KM2O4 solution, producing Fe* and Mn²+ ions in acidic solution. If it required 42.41 mL o 0.0452 M KMNO4 to titrate a solution made from 1.236 g of iron ore, what is the mass percent of iron in the iron ore? Mass percent

The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe+ ions. This solution is then titrated with KM2O4 solution, producing Fe* and Mn²+ ions in acidic solution. If it required 42.41 mL o 0.0452 M KMNO4 to titrate a solution made from 1.236 g of iron ore, what is the mass percent of iron in the iron ore? Mass percent

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...

See similar textbooks

Similar questions

A sample of iron ore weighing 0.962 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required 32.32 mL of 0.0475M KMnO4 for titration. Fill in the table and calculate the % by mass of iron in the ore. Balance the equation: Fe +2 + MnO4 → Fe+3 + MnO2 Computation Name of analyte Iron ore Mass of analyte 0.2792 g Name of titrant KMnO4 Volume of titrant 23.30 mL Milliequivalents of the titrant 2.260 milliequivalents Mass of the analyte 0.125 g % Fe in analyte 44.81%
Formation of bromine from bromide. Assign oxidation numbers to each atom. Identify the oxidizing agent and the reducing agent. 2 Br-(aq) + Mn02(s) + 4 H1+(aq)→ Br2(s) + Mn²*(aq) + 2 H20(I)
An aqueous solution of potassium permanganate KMnO4 is mixed with an aqueous solution of manganese (II) sulfate MnSO4.Justify that a redox reaction is possible and write the equation corresponding to this reaction.
A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?
A 0.8040-g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated with 47.22 mL of 0.02242 M KMn 04 solution. Calculat the results of this analysis in terms of % Fe (55.847 g/mol).
After reducing a 0.4080 g iron to Fe²⁺, it was titrated with 42.72 mL of 0.1211 N KMnO₄ solution. Calculate the percent Fe₃O₄ (231.54 g/mol). The reaction is described by the equation: MnO₄- + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O * Choices 50.81% 70.81% 36.77% 97.86% 58.72%
An aqueous solution of NaCl was electrolyzed with a current of 2.50 amps for 15.0 minutes. What volume (in mL) of 0.500 M HCl would be required to neutralize the resulting solution? (Hint: H2 is produced at the cathode and Cl2 at the anode.)
For the reaction KClO4⟶KCl+2O2 assign oxidation numbers to each element on each side of the equation.
lead + nickel (II) nitrate;Balanced chemical equation:Reaction type:
Balance the following oxidation-reduction reactions. acidic solution a. PbO₂+ Hg-Hg2+ Pb²+ b. NO3(aq) + H2(g) → NO) + H₂O(1) basic solution
A. Balance the following redox reactions using the half-reaction method. B. Identify the oxidizing agent and the reducing agent. 1. Zn(s) + Fe²+ (aq) → Zn²+ (aq) + Fe (s) 2+ Zn(s) → Zn² +2e- oxidiation haut reaction (aq) 2+ 20+ Fe (an) → Fe (5) Reducation haut reaction (94) - Bris) Reducing agent (S) Fe 2+ oxidizing agent 2. (Balance this reaction In Acidic Solution):
Balance the equation ( Oxidation Reduction ): Fe* + MnO4" Mn2+ Fe3