An aqueous solution of acetic acid is found to havethe following equilibrium concentrations at 25 °C:[CH3COOH] = 1.65 x 10-2 M; [H+] = 5.44 x 10-4 M; and[CH3COO-] = 5.44 * 10-4 M. Calculate the equilibriumconstant Kc for the ionization of acetic acid at 25 °C. Thereaction isCH3COOH(aq) ⇌ H+(aq) + CH3COO-(aq)
An aqueous solution of acetic acid is found to havethe following equilibrium concentrations at 25 °C:[CH3COOH] = 1.65 x 10-2 M; [H+] = 5.44 x 10-4 M; and[CH3COO-] = 5.44 * 10-4 M. Calculate the equilibriumconstant Kc for the ionization of acetic acid at 25 °C. Thereaction isCH3COOH(aq) ⇌ H+(aq) + CH3COO-(aq)
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.29P: 7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its...
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An aqueous solution of acetic acid is found to have
the following equilibrium concentrations at 25 °C:
[CH3COOH] = 1.65 x 10-2 M; [H+] = 5.44 x 10-4 M; and
[CH3COO-] = 5.44 * 10-4 M. Calculate the equilibrium
constant Kc for the ionization of acetic acid at 25 °C. The
reaction is
CH3COOH(aq) ⇌ H+(aq) + CH3COO-(aq)
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