A 25.00-mL sample of HCl(aq) was added to a 0.1000-g sample of CaCO3 (100.09 g/mol). All the CaCO3 reacted, leaving some excess HCl(aq), according to [CaCO3(s) + 2HCl -> CaCl2(aq) + H2O(l) + CO2(g)]. The excess HCl(aq) required 43.82 mL of 0.01185 M Ba(OH)2 in a back-titration step to complete the reaction [2HCl(aq) + Ba(OH)2(aq) -> BaCl2(aq) + 2H2O(l)]. What is the molarity of the original HCl(aq) solution?

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 25.00-mL sample of HCl(aq) was added to a 0.1000-g sample of CaCO₃ (100.09 g/mol). All the CaCO₃ reacted, leaving some excess HCl(aq), according to [CaCO₃(s) + 2HCl -> CaCl₂(aq) + H₂O(l) + CO₂(g)]. The excess HCl(aq) required 43.82 mL of 0.01185 M Ba(OH)₂ in a back-titration step to complete the reaction [2HCl(aq) + Ba(OH)₂(aq) -> BaCl₂(aq) + 2H₂O(l)]. What is the molarity of the original HCl(aq) solution?

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