Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![For a solution of 0.020 M lactic acid, HC₃H₅O₂ (Kₐ = 8.4 × 10⁻⁴), calculate:
(a) [H⁺]
[Information box] ___________ M
(b) pH
[Information box] ___________
(c) percent ionization
[Information box] ___________ %](https://content.bartleby.com/qna-images/question/738db1e2-4aa5-4874-9af6-830a7bc8f2f5/3400e5da-156e-41df-b10b-8b725bf513fb/3onghuu_processed.jpeg)
Transcribed Image Text:For a solution of 0.020 M lactic acid, HC₃H₅O₂ (Kₐ = 8.4 × 10⁻⁴), calculate:
(a) [H⁺]
[Information box] ___________ M
(b) pH
[Information box] ___________
(c) percent ionization
[Information box] ___________ %
Expert Solution
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Step 1
Given that: Concentration of lactic acid = 0.020 M and Ka = 8.4×10-4
To find:
- Concentration of H+ ions
- pH of the solution
- Percent ionization
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Step 2
Lactic acid is a weak acid. The dissociation of this weak acid in water is as given by the reaction shown below.
HC3H5O3(aq)→C3H5O−3(aq)+H+(aq)
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Step 3
Let x amount of lactic acid dissociate at equilibrium, the ICE table for the reaction is given by,
HC3H5O3→C3H5O−3+H+I0.02000C−x+x+xE0.020−xxx
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