2.00 g of limestone was dissolved in hydrochloric acid and all the calcium present in the sample was converted to Ca2+. Excess ammonium oxalate solution, (NH4)2C2O4, was added to the solution to precipitate the calcium ions as calcium oxalate, CaC2O4.The precipitate was weighed to a constant mass of 2.43 g. Calculate the percentage by mass of calcium in the limestone.
2.00 g of limestone was dissolved in hydrochloric acid and all the calcium present in the sample was converted to Ca2+. Excess ammonium oxalate solution, (NH4)2C2O4, was added to the solution to precipitate the calcium ions as calcium oxalate, CaC2O4.The precipitate was weighed to a constant mass of 2.43 g. Calculate the percentage by mass of calcium in the limestone.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter4: Chemical Reactions
Section: Chapter Questions
Problem 4.88QP: A 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a...
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2.00 g of limestone was dissolved in hydrochloric acid and all the calcium present in the sample was converted to Ca2+. Excess ammonium oxalate solution, (NH4)2C2O4, was added to the solution to precipitate the calcium ions as calcium oxalate, CaC2O4.The precipitate was weighed to a constant mass of 2.43 g. Calculate the percentage by mass of calcium in the limestone.
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