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An iron ore was analyzed by dissolving a 2.9912-g sample in concentrated HCI. The resulting solution was diluted with water, and the iron(II) was precipitated as the hydrous oxide Fe203-XH2O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.8394 g of pure Fe203 (159.69 g/mol).

An iron ore was analyzed by dissolving a 2.9912-g sample in concentrated HCI. The resulting solution was diluted with water, and the iron(II) was precipitated as the hydrous oxide Fe203-XH2O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.8394 g of pure Fe203 (159.69 g/mol).

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 78QAP: When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white...
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An iron ore was analyzed by dissolving a 2.9912-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe203-xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.8394 g of pure Fe203 (159.69 g/mol). How many grams of Fe (55.847 g/mol) are there in the iron ore sample? 0.2936 g Fe 0.5871 g Fe (C) 0.1468 g Fe D) 0.7739 g Fe
Transcribed Image Text:An iron ore was analyzed by dissolving a 2.9912-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe203-xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.8394 g of pure Fe203 (159.69 g/mol). How many grams of Fe (55.847 g/mol) are there in the iron ore sample? 0.2936 g Fe 0.5871 g Fe (C) 0.1468 g Fe D) 0.7739 g Fe
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