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.
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.
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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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.
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