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How much moles of precipitate was formed? * Probable atomic weights: Ca = 40; C = 12; 0 = 16 Your answer How many moles of calcium are in calcium oxalate? * Your answer * What is the mass (g) of calcium ions in the sample? * Your answer What is the percentage of calcium in the original limestone sample? * Use the COMPLETE computed value for E to compute for the percentage.

How much moles of precipitate was formed? * Probable atomic weights: Ca = 40; C = 12; 0 = 16 Your answer How many moles of calcium are in calcium oxalate? * Your answer * What is the mass (g) of calcium ions in the sample? * Your answer What is the percentage of calcium in the original limestone sample? * Use the COMPLETE computed value for E to compute for the percentage.

General Chemistry - Standalone book (MindTap Course List)
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 4.116QP: Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride,...
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A 2.89 g sample of limestone (CaCO3) was dissolved in 0.12M (HCI) solution according to the following equation: CaCO3 (s) + 2HCI (aq) → Ca²+ (aq) + 2Cl(aq) + CO2(g) + H₂O(1) Excess 0.1M (NH4)2C2O4(aq), was added to the resulting solution to precipitate the calcium ions as calcium oxalate, CaC₂O4(s). The precipitate was filtered, dried, and weighed at 1.75 g.
Transcribed Image Text:A 2.89 g sample of limestone (CaCO3) was dissolved in 0.12M (HCI) solution according to the following equation: CaCO3 (s) + 2HCI (aq) → Ca²+ (aq) + 2Cl(aq) + CO2(g) + H₂O(1) Excess 0.1M (NH4)2C2O4(aq), was added to the resulting solution to precipitate the calcium ions as calcium oxalate, CaC₂O4(s). The precipitate was filtered, dried, and weighed at 1.75 g.
How much moles of precipitate was formed? * Probable atomic weights: Ca = 40; C = 12; 0 = 16 Your answer How many moles of calcium are in calcium oxalate? * Your answer What is the mass (g) of calcium ions in the sample? * Your answer What is the percentage of calcium in the original limestone sample? * Use the COMPLETE computed value for E to compute for the percentage. Your answer
Transcribed Image Text:How much moles of precipitate was formed? * Probable atomic weights: Ca = 40; C = 12; 0 = 16 Your answer How many moles of calcium are in calcium oxalate? * Your answer What is the mass (g) of calcium ions in the sample? * Your answer What is the percentage of calcium in the original limestone sample? * Use the COMPLETE computed value for E to compute for the percentage. Your answer
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