6. A sample of hydrochloric acid is standardized using sodium bicarbonate. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bi- carbonate, NaHCO,. a. ment Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. c. Calculate the mass percent concentration of hydrochloric acid using the molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL. с.

6. A sample of hydrochloric acid is standardized using sodium bicarbonate. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bi- carbonate, NaHCO,. a. ment Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. c. Calculate the mass percent concentration of hydrochloric acid using the molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL. с.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

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