Question
Asked Nov 23, 2019
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Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC2H3O2(aq) + H2O(l) ↔ C2H3O2-(aq) + H3O+(aq). At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: [HC2H3O2]=0.0990 and [C2H3O2-]=1.33×10-3M, and [H3O+]=1.33×10-3M,. The equilibrium constant, Keq, for the ionization of acetic acid at 25 °C is __________.

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Expert Answer

Step 1

The equilibrium constant of a reaction is calculated by the help of equilibrium concentrations of the components and their stoichiometric coefficients.

Step 2

Given data:

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[нC, Н.О,]-0.0990м [сно]-1.33х10 м [н,о1-1.33х10-м

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Step 3

The dissociation reaction of acetic acid i...

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HC,H,O, (a)+HO(1)->C,H,O5(aq)+H,0* (a)

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