All iron in 4.00 g of iron ore sample, which was dissolved in an acid solution, was converted to Fe2+ which was then titrated with 0.200 M KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4 to Mn²*. If 27.45 mL of KMNO4 solution is required to the end point, determine 1. How many grams of iron content is in the iron ore sample. 2. The yield percentage of iron in the sample. 3. If the iron in the sample is present as Fe2O3, what is the mass percentage of Fe2O3 in the sample.

All iron in 4.00 g of iron ore sample, which was dissolved in an acid solution, was converted to Fe2+ which was then titrated with 0.200 M KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4 to Mn²*. If 27.45 mL of KMNO4 solution is required to the end point, determine 1. How many grams of iron content is in the iron ore sample. 2. The yield percentage of iron in the sample. 3. If the iron in the sample is present as Fe2O3, what is the mass percentage of Fe2O3 in the sample.

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

DETERMINE WHETHER THE STATEMENT IS TRUE OR FALSE TRUE OR FALSE 1 In the analysis of Group II Cations, magnesium ribbons must first be dissolved before proceeding with the test for Tin ions.2 In the analysis of Group II cations, Pb⁺² is precipitated as PbSO₄. 3 Cadmium ions precipitate as cadmium hydroxide with hydrogen sulfide. 4 All group IIA cations are oxidized by dilute nitric acid. 5 Cyanide ion forms an unstable colorless complex with copper ions.
A 1.362 g sample of an iron ore that contained FegO4was dissolved in acid and all of the iron was reduced to Fe2*. The solution was then acidified with H2SO4and titrated with 39.42 mL of 0.0281 M KMNO4, which oxidized the iron to Fe. The net ionic equation for the reaction is 5FE2+ + MnO4+8H* 5FE3+ + Mn2+ + 4H2O What was the percentage by mass of iron in the ore? What was the percentage by mass of FegO4 in the ore? Part 1 Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used Part 2 Using the previous answer and the balanced equation, find the number of moles of Fe2+. mol Fe2+
You are tasked with creating a pourboix diagram of copper speciation. The relevent species are Cu 1+, Cu 2+, Cu2O, and CuO. The total copper is 10^-3 mol. Set and balence the redox reactions needed for this question and explain how you landed on those reactions.
Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H 2C 2O 4 and H 2O in the balanced reaction? MnO 4⁻( aq) + H 2C 2O 4( aq) → Mn 2+( aq) + CO 2( g) H2C2O4 = 5, H2O = 8 H2C2O4 = 1, H2O = 4 H2C2O4 = 5, H2O = 1 H2C2O4 = 1, H2O = 1 H2C2O4 = 3, H2O = 2
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%
Balance the following reaction in acidic solution. Cr2O, (ag) + HNO,(aq) → Cr* (aq) + NO, (aq) 3 Fill in the coefficients for the balanced overall equation. HNO, + -- v H* + -v Cr.O,* → -- ♥ NO, +- Cr3+ + Cr,O, - H.O --V
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)
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%
4. Balance the following (redox) chemical equations using the half-reaction method, assuming acidic conditions: a. Br(aq) + NO2(aq) → Br2(aq) + NO(g) b. H2O2(aq) + S²(aq) → H2O(1) + S(s) c. Cu(s) + NO3(aq) → Cu²*(aq) + NO2(g)
The blood alcohol C2 H; OH level can be determined by titrating a sample of blood plasma with an acidic potassium dichromate solution, resulting in the production of Cr*+ (aq) and carbon dioxide. The reaction can be monitored because the dichromate ion (Cr2 O,²) is orange in solution, and the Cr³* ion is green. The unbalanced redox equation is Cr2 O,2 (aq) + C2H; OH(ag) → Cr³* (ag) + CO2 (g) If 40.35 mL of 0.0711 M potassium dichromate solution is required to titrate 27.5 g of blood plasma, determine the mass percent of alcohol in the blood. Mass percent
24. A sample of iron ore (0.2482 g) was dissolved in an excess of a dilute acid solution. All of the iron was first converted to the Iron (II) ion. The solution then required 26.89 mL of a 0.0250 M KMNO4 for oxidation to the Iron (III) ion. What is the mass percent of iron in the ore? 2+
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 Fe2+ ions. This solution is then titrated with KMn04 solution, producing Fe3+ and Mn2+ ions in acidic solution. Ifit required 38.37 mL of 0.0198 M KMnO4 to titrate a solution made from 0.6128 g of iron ore, what is the mass percent of iron in the iron ore?