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A solution contains 0.2 mol/l of the salt ammonium acetate (NH+4CH3COO-). The pH of the solution has been adjusted to 8.0 via addition of NaOH. The equilibrium constants for the deprotonation of acetic acid and the ammonium ion are: NH+4(aq)+H2O(l) = NH3(aq)+H3O+(aq) pKa1=9.25 CH3COOH(aq)+H2O(1)= CH3COO-(aq)+H3O+(aq) pKa2=4.75 1. Calculate the concentration of ammonia (NH3NH3) in the solution. 2. Calculate the concentration of acetate ions (CH3COO-CH3COO-) in the solution. 3. Calculate the concentration of non-dissociated acetic acid (CH3COOHCH3COOH) in the solution. 4. Calculate the concentration of sodium ions in the solution. 5. Calculate the pH of a solution containing the same amount of NaOH in absence of ammonium acetate. 6. Calculate the pH of a 0.2 mol/l ammonium acetate solution, if no NaOH is added.

A solution contains 0.2 mol/l of the salt ammonium acetate (NH+4CH3COO-). The pH of the solution has been adjusted to 8.0 via addition of NaOH. The equilibrium constants for the deprotonation of acetic acid and the ammonium ion are: NH+4(aq)+H2O(l) = NH3(aq)+H3O+(aq) pKa1=9.25 CH3COOH(aq)+H2O(1)= CH3COO-(aq)+H3O+(aq) pKa2=4.75 1. Calculate the concentration of ammonia (NH3NH3) in the solution. 2. Calculate the concentration of acetate ions (CH3COO-CH3COO-) in the solution. 3. Calculate the concentration of non-dissociated acetic acid (CH3COOHCH3COOH) in the solution. 4. Calculate the concentration of sodium ions in the solution. 5. Calculate the pH of a solution containing the same amount of NaOH in absence of ammonium acetate. 6. Calculate the pH of a 0.2 mol/l ammonium acetate solution, if no NaOH is added.

Chemistry
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 solution contains 0.2 mol/l of the salt ammonium acetate (NH+4CH3COO-). The pH of the solution has been adjusted to 8.0 via addition of NaOH. The equilibrium constants for the deprotonation of acetic acid and the ammonium ion are: NH+4(aq)+H2O(l) = NH3(aq)+H3O+(aq) pKa1=9.25 CH3COOH(aq)+H2O(1)= CH3COO-(aq)+H3O+(aq) pKa2=4.75 1. Calculate the concentration of ammonia (NH3NH3) in the solution. 2. Calculate the concentration of acetate ions (CH3COO-CH3COO-) in the solution. 3. Calculate the concentration of non-dissociated acetic acid (CH3COOHCH3COOH) in the solution. 4. Calculate the concentration of sodium ions in the solution. 5. Calculate the pH of a solution containing the same amount of NaOH in absence of ammonium acetate. 6. Calculate the pH of a 0.2 mol/l ammonium acetate solution, if no NaOH is added.
Transcribed Image Text:A solution contains 0.2 mol/l of the salt ammonium acetate (NH+4CH3COO-). The pH of the solution has been adjusted to 8.0 via addition of NaOH. The equilibrium constants for the deprotonation of acetic acid and the ammonium ion are: NH+4(aq)+H2O(l) = NH3(aq)+H3O+(aq) pKa1=9.25 CH3COOH(aq)+H2O(1)= CH3COO-(aq)+H3O+(aq) pKa2=4.75 1. Calculate the concentration of ammonia (NH3NH3) in the solution. 2. Calculate the concentration of acetate ions (CH3COO-CH3COO-) in the solution. 3. Calculate the concentration of non-dissociated acetic acid (CH3COOHCH3COOH) in the solution. 4. Calculate the concentration of sodium ions in the solution. 5. Calculate the pH of a solution containing the same amount of NaOH in absence of ammonium acetate. 6. Calculate the pH of a 0.2 mol/l ammonium acetate solution, if no NaOH is added.
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