I need the answer as soon as possible Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. Thesolution was diluted in H,O, Fe() was precipitated as Fe,O3 H2O by adding NH3.After filteration, washing the residue ignited to give 0 2697 g of pure Fe203(159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample.avedput of69.12 %O 54.21 %O 33.32 %16.66 %O 45.21 %

Given: Mass of iron sample = 1.1324 g Mass of Fe2O3 produced = 0.2697 g

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. The solution was diluted in H,O, Fe() was precipitated as Fe203 H2O by adding NH3. After filteration, washing the residue ignited to give 0.2697 g of pure Fe203 (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. 69.12 % O 54.21 % O 33.32 % O 16.66 % O 45.21 %

Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL. The solution was diluted in H,O, Fe() was precipitated as Fe203 H2O by adding NH3. After filteration, washing the residue ignited to give 0.2697 g of pure Fe203 (159.69 g/mol). Calculate %Fe (55.847g/mol) in the sample. 69.12 % O 54.21 % O 33.32 % O 16.66 % O 45.21 %

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter12: Gravimetric Methods Of Analysis

Section: Chapter Questions

Problem 12.20QAP

See similar textbooks

Similar questions

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?
The aluminum in 0.200 g impure aluminum sulfate ( the sample) was precipitated with aqueous NH3and the precipitate was filtered and ignited to 10000C to give anhydrous Al2O3 (the residue) which weighs 0.150 g. Calculate the %Al ( the %sfc) in the sample.
1,5419 g of magnetite (Fe3O4) ore; Fe+2 and Fe + 3 in concentrated HCL to form a mixtureit's unraveling. Adding HNO3 to all Fe +2s Fe +3 e and Fe+3 s NH, addingwith Fe(OH)3, precipitating into. Sediment in the form of Fe3O4 after necessary operationsand 0.8525 g. Calculate the percentage of Fe3O4 in the sample.
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.
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 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.
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)
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 0.7352g sample of ore containing Fe3+, Al3+ and Sr2+ was dissolved and made up to 500.00 mL. The analysis of metals was performed by a chemistry using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard solution of EDTA 0.02145 mol/L, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Determine the percentage of each of the metals in the sample Given the molar masses: Fe=55.845 g/mol; Al=26.982 g/mol and Sr=87.620 g/mol.
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 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