A 0.450 g sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO3(s) + 2HCl(aq) - CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 5.60 mL of 0.125 M NaOH(aq). Calculate the mass percentage of CaCO3(s) in the sample. mass percentage:
A 0.450 g sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO3(s) + 2HCl(aq) - CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 5.60 mL of 0.125 M NaOH(aq). Calculate the mass percentage of CaCO3(s) in the sample. mass percentage:
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 59QAP: In order to determine the purity of ammonium sulfate, a sample with a mass of 0.850 g is dissolved...
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![A 0.450 g sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq).
The equation for the reaction is
CaCO3(s) + 2HCl(aq)
-
CaCl2(aq) + H2O(l) + CO2(g)
The excess HCl(aq) is titrated by 5.60 mL of 0.125 M NaOH(aq).
Calculate the mass percentage of CaCO3(s) in the sample.
mass percentage:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8deec336-4294-4d46-88c2-8705159595da%2Fcee11d3a-668c-40b6-9d42-fe92f24d1dca%2Fmugmxc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 0.450 g sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq).
The equation for the reaction is
CaCO3(s) + 2HCl(aq)
-
CaCl2(aq) + H2O(l) + CO2(g)
The excess HCl(aq) is titrated by 5.60 mL of 0.125 M NaOH(aq).
Calculate the mass percentage of CaCO3(s) in the sample.
mass percentage:
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