2. You are measuring the Fe(II) content of a sample of FeCl2.4H20. You weighed out1.20g FeCl2.4H20 and dissolved it in 50 mls of 0.5M sulfuric acid. You removed 10ml.s of this solution, mixed it with sulfuric acid and diphenylamine sulfonateindicator, and titrated it to the equivalence point with 0.0167M K2Cr207 solution.You obtained the following data.Volume of dichromate needed to reach the equiv. point = 9.5 ml.sGiven that MeVEe = 6MaiVdi, (where Mre= molarity of the Fe(II) solution, Vre is thevolume of the Fe(II) solution =10 mls. Mai = molarity of the dichromate solution-0.0167M, and Vai = volume of dichromatsolution = 9.5 ml.s), calculate:%3D(a) The molarity of the Fe(Il) solution-M(b) Mass of Fe in the original solution = (Me)(0.05)(55.845) = ------(c) The theoretical mass % Fe in FeCl2.4H20 - -%(d) The experimental mass % Fe in your sample of FeCl2.4H2O----%(e) The % error in your determination of the mass % Fe ---------%

2. You are measuring the Fe(lI) content of a sample of FeCl2.4H20. You weighed out 1.20g FeCl2.4H20 and dissolved it in 50 ml.s of 0.5M sulfuric acid. You removed 10 ml.s of this solution, mixed it with sulfuric acid and diphenylamine sulfonate indicator, and titrated it to the equivalence point with 0.0167M K2Cr207 solution. You obtained the following data. Volume of dichromate needed to reach the equiv. point = 9.5 ml.s Given that MEeVFe 6MaiVai, (where Mre= molarity of the Fe(lI) solution, VEe is the volume of the Fe(II) solution =10 mls. Mai= molarity of the dichromate solution 0.0167M, and Vdi = volume of dichromat solution = 9.5 ml.s), calculate: %3D %3D %3D (a) The molarity of the Fe(Il) solution ----------M (b) Mass of Fe in the original solution = (MF)(0.05)(55.845) = (c) The theoretical mass % Fe in FeCl2.4H20 -----%

2. You are measuring the Fe(lI) content of a sample of FeCl2.4H20. You weighed out 1.20g FeCl2.4H20 and dissolved it in 50 ml.s of 0.5M sulfuric acid. You removed 10 ml.s of this solution, mixed it with sulfuric acid and diphenylamine sulfonate indicator, and titrated it to the equivalence point with 0.0167M K2Cr207 solution. You obtained the following data. Volume of dichromate needed to reach the equiv. point = 9.5 ml.s Given that MEeVFe 6MaiVai, (where Mre= molarity of the Fe(lI) solution, VEe is the volume of the Fe(II) solution =10 mls. Mai= molarity of the dichromate solution 0.0167M, and Vdi = volume of dichromat solution = 9.5 ml.s), calculate: %3D %3D %3D (a) The molarity of the Fe(Il) solution ----------M (b) Mass of Fe in the original solution = (MF)(0.05)(55.845) = (c) The theoretical mass % Fe in FeCl2.4H20 -----%

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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A quantitative analysis for ethanol, C2H60, is accomplished by a redox back titration. Ethanol is oxidized to acetic acid, C2H402, using excess dichromate, 3+ Cr207 2-, which is reduced to Cr3*. The excess dichromate is titrated with Fe2*, giving C and Fe+ as products. In a typical analysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mL sample is taken and the ethanol is removed by distillation and collected in 50.00 mL of an 2- acidified solution of 0.0200 M K2Cr207. Titration of the unreacted Cr207 requires 21.48 mL of 0.1014 M Fe2*. Calculate the %w/v ethanol in the brandy. Which is the titrant in this problem? C2H402 Fe2+ C2H60 O Cr207 2-
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