Iron was analyzed by dissolving 1.1324 g sample inconcentrated HCL. The solution was diluted in H20, Fe(II) wasprecipitated as Fe,03.H20 by adding NH3. After filteration,washing the residue ignited to give 0.5394 g of pure Fe203(159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample.O 33.32 %O 69.12 %O 45.21 %O 54.21 %23.21 %

Given: Mass of iron sample = 1.1324 g Mass of Fe2O3 produced = 0.5394 g

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. The solution was diluted in H20, Fe(lII) was precipitated as Fe2O3.H2O by adding NH3. After filteration, washing the residue ignited to give 0.5394 g of pure Fe203 (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. O 33.32 % 69.12 % 45.21 % 54.21 % 23.21 %

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. The solution was diluted in H20, Fe(lII) was precipitated as Fe2O3.H2O by adding NH3. After filteration, washing the residue ignited to give 0.5394 g of pure Fe203 (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. O 33.32 % 69.12 % 45.21 % 54.21 % 23.21 %

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.33QAP

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A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO
A 5.70 g iron ore was dissolved in concentrated HCl. After the dissolution, the resulting solution was made basic by adding 6.0 M NaOH slowly until the solution is slightly turbid. Urea was then added and the solution was heated for 3 hours. The precipitate was filtered using an ashless filter paper and ignited to form Fe2O3 (159.69 g/mol). The mass of precipitate is 2.1 g. Find the % Fe3O4 (231.54 g/mol) in the iron ore sample.
To analyze the amount of iron (Fe; Mw = 55.85 g/mol) contained in an ore sample, the sample was digested with acid and diluted to 50 mL with water. This solution was then treated with 25.00 mL of 0.2922 M EDTA. The excess EDTA was back titrated with 6.47 mL of 0.0843 M Zn2+ to reach the equivalence point. How many grams of Fe contained in the ore sample?
Give only typing answer with explanation and conclusion 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol)
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To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.
A 3.25 g sample of an iron-containing mineral was dissolved in an acid medium and calibrated to 500 mL. A 25.00 mL aliquot was titrated with 0.0025 M KMnO4 spending a volume of 9.32 mL. Subsequently, a 25.00 mL aliquot was passed through a Walden reducer to later titrate it with the same permanganate solution, using a volume of 14.15 mL for the titration. Determine the percentage of Fe(III) in the sample and report it as % Fe2O3
A 5.70 g iron ore was dissolved in concentrated HCL After the dissolution, the resulting solution was made basic by adding 6.0 M NaOH slowly until the solution is slightly turbid. Urea was then added and the solution was heated for 3 hours. The precipitate was filtered using an ashless filter paper and ignited to form Fe2O3 (159.69 L /mol The mass of precipitate is 2.1g. Find the % Fe3O4 (231.54 c/mol) in the iron are sample.
A salt sample was analyzed for its purity. A 0.5000 g sample was dissolved in water and diluted to 250 mL. From this solution, 25.00 mL was taken for analysis. To this aliquot, 20.00 mL of a 0.08735 M AgNO3 solution was added to precipitate the chloride. The excess AgNO3 required 12.45 mL of a 0.09473 M KSCN solution for back-titration. Calculate the purity of the salt sample as percent by mass of KCl (74.55 g/mol)
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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

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