A 0.717 gram sample of an unknown monoprotic acid is dissolved in 40.0 mL of water and titrated with a a 0.221 M aqueous barium hydroxide solution. It is observed that after 8.28 milliliters of barium hydroxide have been added, the pH is 3.465 and that an additional 4.32 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for the acid?
A 0.717 gram sample of an unknown monoprotic acid is dissolved in 40.0 mL of water and titrated with a a 0.221 M aqueous barium hydroxide solution. It is observed that after 8.28 milliliters of barium hydroxide have been added, the pH is 3.465 and that an additional 4.32 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for the acid?
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 57P
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A 0.717 gram sample of an unknown monoprotic acid is dissolved in 40.0 mL of water and titrated with a a 0.221 M aqueous barium hydroxide solution. It is observed that after 8.28 milliliters of barium hydroxide have been added, the pH is 3.465 and that an additional 4.32 mL of the barium hydroxide solution is required to reach the equivalence point.
(1) What is the molecular weight of the acid? g/mol
(2) What is the value of Ka for the acid?
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