Explanation The equilibrium reaction is given below. C H 3 C H 2 C O O H ( a q ) + H 2 O ( l ) ⇌ C H 3 C H 2 C O O − ( a q ) + H 3 O + ( a q ) The acid ionization constant can be written as given below. K a = [ C H 3 C H 2 C O O − ] [ H 3 O + ] [ C H 3 C H 2 C O O H ] A table can be set up as shown below. C H 3 C H 2 C O O H ( a q ) H 3 O + ( a q ) C H 3 C H 2 C O O − ( a q ) I n i t i a l c o n c . ( M ) 0.20 1 × 10 − 7 0 C h a n g e i n c o n c . ( M ) − x + x + x E q u i l i b r i u m c o n c . ( M ) 0.20 − x x x The concentration of H 3 O + comes from its autoionization that is 1.0 × 10 − 7

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ISBN: 9781285199047

Author: John W. Moore, Conrad L. Stanitski

Publisher: Cengage Learning

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Chapter 14, Problem 58QRT

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Interpretation:

The equilibrium concentrations of H3O+, acetate ion and acetic acid in a 0.20 M aqueous solution of acetic acid have to be calculated.

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Chapter 14, Problem 57QRT

Chapter 14, Problem 59QRT

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The equilibrium concentrations of H 3 O + , acetate ion and acetic acid in a 0.20 M aqueous solution of acetic acid have to be calculated.

Solution Summary: The author explains the equilibrium concentrations of H_3O+, acetate ion and acetic acid in an 0.20M solution.

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Interpretation:

The equilibrium concentrations of H3O+, acetate ion and acetic acid in a 0.20 M aqueous solution of acetic acid have to be calculated.

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Chapter 14 Solutions

The equilibrium concentrations of H 3 O + , acetate ion and acetic acid in a 0.20 M aqueous solution of acetic acid have to be calculated.

Solution Summary: The author explains the equilibrium concentrations of H_3O+, acetate ion and acetic acid in an 0.20M solution.

Concept explainers

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Interpretation: The equilibrium concentrations of H3O+, acetate ion and acetic acid in a 0.20 M aqueous solution of acetic acid have to be calculated.

Want to see the full answer?

Chapter 14 Solutions

Interpretation:

The equilibrium concentrations of H3O+, acetate ion and acetic acid in a 0.20 M aqueous solution of acetic acid have to be calculated.