A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe,O3 (a9) to elemental iron. I Enough sulfur trioxide gas was bubbled to Fe,O; aqueous suspension to completely yield ferric sulfate IL Then, 5.00 M nitric acid was added to ferric sulfate yielding aqueous solution of ferric nitrate I Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron. а. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, 1, g). (CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express your answers in 3 significant figures. High-concentration HCl is supposed to be added at the last part of the procedure. с. Briefly state its purpose.

A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe,O3 (a9) to elemental iron. I Enough sulfur trioxide gas was bubbled to Fe,O; aqueous suspension to completely yield ferric sulfate IL Then, 5.00 M nitric acid was added to ferric sulfate yielding aqueous solution of ferric nitrate I Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron. а. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, 1, g). (CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express your answers in 3 significant figures. High-concentration HCl is supposed to be added at the last part of the procedure. с. Briefly state its purpose.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.34QAP

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Consider the electrolysis of a molten salt of some metal. What information must you know to calculate the mass of metal plated out in the electrolytic cell?
Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution. Box the final answer.
7
0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???
1. 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 KMnO4 solution. Calculate the results of this analysis in terms of (a) %Fe (MW = 55.845) and (b) %Fe3O4 (MW = 231.535). Consider the reaction 5 Fe²+ + MnO4 + 8H+ → 5Fe3+ + Mn²+ + 4H₂O
In aqueous solution, hydrogen sulfide reduces (a) Fe3 + toFe2+ , (b) Br2 to Br - , (c) MnO4- to Mn2 + , (d) HNO3 to NO2.In all cases, under appropriate conditions, the product iselemental sulfur. Write a balanced net ionic equation foreach reaction.
A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron. I Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate, II. Then, 5.00 M nitric acid was added to ferric sulfate yielding aqueous solution of ferric nitrate. III Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron.
Accounts for the following(i) Rusting of iron is quicker in saline water than in ordinary water.(ii) Blocks of magnesium are straped to the steel hubs of ocean going ships.
A sample of impure KI weighing 0.600 g is dissolved in water, the solution acidified, and 25.00 mL of 0.0400 M KIO3 (an excess ) is added. The iodate is reduced to I2 and the iodide is oxidized to I, The I2 is boiled off, the solution cooled, and an excess of pure KI is added to react with the unused KIO3. The I2 produced is titrated with 40.38 mL of 0.1053 N thiosulfate. Write the equations for the reactions which occurred and calculate the percentage of KI in the sample.
Complete and balance the following equations for reac- tions taking place in basic solution. (a) Cr(OH);(s) + Brz (aq) - (b) ZrO(OH)2(s) + SO3 (aq) → (c) HP6O5(aq) + Re(s) - (d) HXeO, (aq)· (e) N,H4(aq)+ CO; (aq) → N2(g)+ CO(g) - Cro (aq) + Br (aq) Zr(s) + SO¯ (aq) → Pb(s) + ReO, (aq) → XeO-(aq) + Xe(g) -
The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?

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