A 1.00 M solution of fluoroacetic acid is 10.0% dissociated in water at a certain temperature. The dissociation is shown below. FCH:COOH + H20 = FCH2CO0- + H3O* 1. After dissociation, what will be the equilibrium concentration of FCH;COOH? 1.617 M None of the choices 299.5 M 0.050 M 1.617 x 10-4 M 2. After dissociation, what will be the equilibrium concentration of FCH2C00-? 0.050 M 0.50 M 0.010 M 0.10 M None of the choices 3. After dissociation, what will be the equilibrium concentration of H3O*? 0.010 M 0.50 M None of the choices 0.10 M 0.050 M

A 1.00 M solution of fluoroacetic acid is 10.0% dissociated in water at a certain temperature. The dissociation is shown below. FCH:COOH + H20 = FCH2CO0- + H3O* 1. After dissociation, what will be the equilibrium concentration of FCH;COOH? 1.617 M None of the choices 299.5 M 0.050 M 1.617 x 10-4 M 2. After dissociation, what will be the equilibrium concentration of FCH2C00-? 0.050 M 0.50 M 0.010 M 0.10 M None of the choices 3. After dissociation, what will be the equilibrium concentration of H3O*? 0.010 M 0.50 M None of the choices 0.10 M 0.050 M

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 175CP: Calculate the pH of a 0.200-M solution of C5H5NHF. Hint: C5H5NHF is a salt composed of C5H5NH+ and F...

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