A volume of 0.300 L contains, in addition to water, also 0.250 M acetic acid and 0.560 M sodium acetate. 3 mL of 2 M hydrochloric acid (0.0060 mol hydrochloric acid) is added to this buffer. a) Calculate the pH of the original solution using Henderson-Hasselbalchs equation. pKa (CH3COOH) = 4.75 b) Calculate the pH of the original solution based on the equilibrium that actually occurs in the solution. The experimental acid equilibrium constant for acetic acid, Ka = 1.80 x 10-5 c) How well the pH calculated in (a) and (b) matches. If there is a difference, what is it? on? What is your conclusion about when it is appropriate to use Henderson-Hasselbalchs the equation? d) What is the pH of the new solution, after the addition of hydrochloric acid?
A volume of 0.300 L contains, in addition to water, also 0.250 M acetic acid and 0.560 M sodium acetate. 3 mL of 2 M hydrochloric acid (0.0060 mol hydrochloric acid) is added to this buffer. a) Calculate the pH of the original solution using Henderson-Hasselbalchs equation. pKa (CH3COOH) = 4.75 b) Calculate the pH of the original solution based on the equilibrium that actually occurs in the solution. The experimental acid equilibrium constant for acetic acid, Ka = 1.80 x 10-5 c) How well the pH calculated in (a) and (b) matches. If there is a difference, what is it? on? What is your conclusion about when it is appropriate to use Henderson-Hasselbalchs the equation? d) What is the pH of the new solution, after the addition of hydrochloric acid?
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 112CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...
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A volume of 0.300 L contains, in addition to water, also 0.250 M acetic acid and 0.560 M
sodium acetate. 3 mL of 2 M hydrochloric acid (0.0060 mol hydrochloric acid) is added to this buffer.
a) Calculate the pH of the original solution using Henderson-Hasselbalchs
equation. pKa (CH3COOH) = 4.75
b) Calculate the pH of the original solution based on the equilibrium that actually occurs
in the solution. The experimental acid equilibrium constant for acetic acid, Ka = 1.80 x 10-5
c) How well the pH calculated in (a) and (b) matches. If there is a difference, what is it?
on? What is your conclusion about when it is appropriate to use Henderson-Hasselbalchs
the equation?
d) What is the pH of the new solution, after the addition of hydrochloric acid?
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Step 1: Introduction
VIEWStep 2: Calculating the pH of the original solution using Henderson-Hasselbalch's Equation.
VIEWStep 3: Calculating the pH of the original solution based on the Equilibrium that actually occurs.
VIEWStep 4: Analyze the difference in the pH calculated in (a) and (b)
VIEWStep 5: Calculating the pH of the new solution after the addition of 0.0060 mol HCl.
VIEWStep 6: Contd.. Calculating the pH of the new solution after the addition of 0.0060 mol HCl.
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