A 0.804 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.465 M aqueous barium hydroxide solution. It is observed that after 2.54 milliliters of barium hydroxide have been added, the pH is 3.089 and that an additional 4.21 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of Ka for the acid? g/mol

A 0.804 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.465 M aqueous barium hydroxide solution. It is observed that after 2.54 milliliters of barium hydroxide have been added, the pH is 3.089 and that an additional 4.21 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of Ka for the acid? g/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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