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An aqueous solution of CH3COOH is found to have the following equilibrium concentrations at 25°C: CH3COOH =1.65c10 2 M Ht=5.44x10 4 M CH3COO = 5.44c10-4 M Calculate the equilibrium constant, Kc, for the ionization of acetic acid at 25°C. The reaction is CH3COOH(aq) =H"(aq) + CH;COO (aq) Type the numerical value only in two significant figures.

An aqueous solution of CH3COOH is found to have the following equilibrium concentrations at 25°C: CH3COOH =1.65c10 2 M Ht=5.44x10 4 M CH3COO = 5.44c10-4 M Calculate the equilibrium constant, Kc, for the ionization of acetic acid at 25°C. The reaction is CH3COOH(aq) =H"(aq) + CH;COO (aq) Type the numerical value only in two significant figures.

Introduction to General, Organic and Biochemistry
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 CH3COOH is found to have the following equilibrium concentrations at 25°C: CH3COOH = 1.65a102 M Ht= 5.44x10-4 M CH COO = 5.44x10 4 M Calculate the equilibrium constant, Kc, for the ionization of acetic acid at 25°C. The reaction is CH3COOH(aq) = H(aq) + CH;COO (aq) Type the numerical value only in two significant figures.
Transcribed Image Text:An aqueous solution of CH3COOH is found to have the following equilibrium concentrations at 25°C: CH3COOH = 1.65a102 M Ht= 5.44x10-4 M CH COO = 5.44x10 4 M Calculate the equilibrium constant, Kc, for the ionization of acetic acid at 25°C. The reaction is CH3COOH(aq) = H(aq) + CH;COO (aq) Type the numerical value only in two significant figures.
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