Fe (55.85 g/mol) is precipitated as Fe(OH)3 (106.87 g/mol) which is typically ignited to form Fe2O3 (159.69 g/mol) prior to weighing. The Fe in a 2.00 L solution was precipitated and ignited, yielding 0.57 g of Fe2O3. Calculate the original ppm.
Fe (55.85 g/mol) is precipitated as Fe(OH)3 (106.87 g/mol) which is typically ignited to form Fe2O3 (159.69 g/mol) prior to weighing. The Fe in a 2.00 L solution was precipitated and ignited, yielding 0.57 g of Fe2O3. Calculate the original ppm.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability
Section20.7: Green Chemistry And Sustainability
Problem 2.1ACP: Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the...
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Fe (55.85 g/mol) is precipitated as Fe(OH)3 (106.87 g/mol) which is typically ignited to form Fe2O3 (159.69 g/mol) prior to weighing. The Fe in a 2.00 L solution was precipitated and ignited, yielding 0.57 g of Fe2O3. Calculate the original ppm.
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