A sample of steel weighing 2.00 g is analyzed for Cr (AW 52.0). The Cr is oxidized into chromate with alkaline permanganate and the excess permanganate is destroyed. A certain volume of 0.120 M FESO4 is added to the acid solution and the excess is titrated with 0.0220 M KMNO4, requiring 31.0 mL. If the sample contained 0.50 % Cr, what volume (in mL) of FeSO4 was added? Type your numerical answer in the space provided. Do not include the unit. Answer in 3 significant figures. Type your answer.

A sample of steel weighing 2.00 g is analyzed for Cr (AW 52.0). The Cr is oxidized into chromate with alkaline permanganate and the excess permanganate is destroyed. A certain volume of 0.120 M FESO4 is added to the acid solution and the excess is titrated with 0.0220 M KMNO4, requiring 31.0 mL. If the sample contained 0.50 % Cr, what volume (in mL) of FeSO4 was added? Type your numerical answer in the space provided. Do not include the unit. Answer in 3 significant figures. Type your answer.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter20: Chemistry Of The Metals

Section: Chapter Questions

Problem 43QAP

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A sample of steel weighing 2.00 g is analyzed for Cr (AW 52.0). The Cr is oxidized into chromate with alkaline permanganate and the excess permanganate is destroyed. A certain volume of 0.120 M FeSO, is added to the acid solution and the excess is titrated with 0.0220 M KMNO4, requiring 31.0 mL. If the sample contained 0.50 % Cr, what volume (in mL) of FeSO, was added?
A sample of steel weighing 2.00 g is analyzed for Cr (AW 52.0). The Cr is oxidized into chromate with alkaline permanganate and the excess permanganate is destroyed. A certain volume of 0.120 M FeSO4 is added to the acid solution and the excess is titrated with 0.0220 M KMnO4, requiring 31.0 mL. If the sample contained 0.50 % Cr, what volume (in mL) of FeSO4 was added?
A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Calculate the iron content of the ore as%w/w Fe2O3
A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w Fe2O3.
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.
A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.
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
A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid. The Fe3+ is reduced with SnCl2, HgCl2 is adthe Fe2+ titrated with 0.1667 M K2Cr2O7 solution, requiring 12.96 mL. What was the formula of the original oxide? FeO Fe3O4 Fe2O3Fe2O
An alloy containing Ni, Fe and Cr was analyzed by a complexation titration using EDTA as titrant. A 0.7176 g sample of the alloy was dissolved in HNO3 and diluted to 250 mL in a flask. A 50.00 mL aliquot of the sample, treated with pyrophosphate to mask Fe and Cr, required 26.14 mL of 0.05831 M EDTA to reach the murexide endpoint. A second 50.00 mL aliquot was treated with hexamethylenetetramine to mask Cr and titration with 0.05831 M EDTA required 35.43 mL to reach the murexide endpoint. Finally, a third 50.00 mL aliquot was treated with 50.00 mL of 0.05831 M EDTA and titrated back to the murexide endpoint with 6.21 mL of 0.06316 M Cu(II). the weight percentages of Ni, Fe and Cr in the alloy.
A 750.0-mg sample of iron ore was dissolved in acid and treated to oxidize all the iron to ferric ion. After destroying any remaining oxidizing agent, excess KI was added. The liberated I2 required 28.50 mL of 0.07500 M Na2S2O3 for titration. What is the % w/w Fe in the sample? The reactions involved for this titration are the following: 2Fe3+ + I- → 2Fe2+ + I2 I2 + 2S2O32- → 2I- + S4O62-
A 750.0-mg sample of iron ore was dissolved in acid and treated to oxidize all the iron to ferric ion. After destroying any remaining oxidizing agent, excess KI was added. The liberated I2 required 28.50 mL of 0.07500 M Na2S2O3 for titration. What is the % w/w Fe in the sample? The reactions involved for this titration are the following: 2Fe3+ + I- ? 2Fe2+ + I2 I2 + 2S2O32- ? 2I- + S4O62-
The amount of Fe in a 0.4891 gm sample of an ore was determined by redox titration with K Cr , 0 ,. The sample was dissolved in HCl , and the iron brought into ( +2 ) oxidation state . The titration to the end point required 36.92ml of 0.02153 M K Cr , 0 ,. Report the iron content of the ore as % w / w Fe 03 .

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