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In one gravimetric analysis, the iron (Fe) in a 1.6374 g of impure iron compound was dissolved with nitric acid, HNO3 to oxidize iron. The precipitate will be formed as hydrous compound. The precipitate was then filtered, rinsed and ignited at 900°C to give anhydrous Fe₂O3 weighed of 0.8994 g. Calculate the percentage by mass of Fe in a sample

In one gravimetric analysis, the iron (Fe) in a 1.6374 g of impure iron compound was dissolved with nitric acid, HNO3 to oxidize iron. The precipitate will be formed as hydrous compound. The precipitate was then filtered, rinsed and ignited at 900°C to give anhydrous Fe₂O3 weighed of 0.8994 g. Calculate the percentage by mass of Fe in a sample

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter18: Representative Metals, Metalloids, And Nonmetals
Section: Chapter Questions
Problem 25E: A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric...
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In one gravimetric analysis, the iron (Fe) in a 1.6374 g of impure iron compound was dissolved with nitric acid, HNO3 to oxidize iron. The precipitate will be formed as hydrous compound. The precipitate was then filtered, rinsed and ignited at 900°C to give anhydrous Fe2O3 weighed of 0.8994 g. Calculate the percentage by mass of Fe in a sample.
Transcribed Image Text:In one gravimetric analysis, the iron (Fe) in a 1.6374 g of impure iron compound was dissolved with nitric acid, HNO3 to oxidize iron. The precipitate will be formed as hydrous compound. The precipitate was then filtered, rinsed and ignited at 900°C to give anhydrous Fe2O3 weighed of 0.8994 g. Calculate the percentage by mass of Fe in a sample.
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