Acids and Bases
AdvancedAcids and bases are central to chemistry, biology, and environmental science. This topic covers Arrhenius, Bronsted-Lowry, and Lewis definitions. Strong acids dissociate completely; weak acids establish equilibrium described by Ka.
pH quantifies acidity on a logarithmic scale. Buffers resist pH changes using conjugate acid-base pairs and the Henderson-Hasselbalch equation. Titration curves reveal equivalence points and indicator selection.
Covers pH calculations, Ka/Kb, buffers, titrations, polyprotic acids, and Lewis acid-base theory for AP Chemistry Unit 8.
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Learning objectives
- •Calculate pH, pOH, and pKa for strong and weak acid/base solutions
- •Apply Ka and Kb to calculate equilibrium concentrations and percent ionization
- •Design and analyze buffer systems using Henderson-Hasselbalch equation
- •Interpret titration curves for strong/weak acid-base combinations
- •Explain indicator selection based on pKa and equivalence point pH
Recommended Resources
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Books
Chemistry: The Central Science
by Brown, LeMay, Bursten, Murphy
Acids and Bases: A Very Short Introduction
by Oxford University Press
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