Chad provides an introduction to acids and bases beginning with three common definitions for acids and bases: the Arrhenius acid and base, the Bronsted-Lowry acid and base, and the Lewis acid and base. The differences between the definitions are discussed with examples that demonstrate these differences. An Arrhenius acid is an H+ donor in water which increases the concentration of H3O+. An Arrhenius base is an OH- donor in water which increases the OH- concentration in water. A Bronsted-Lowry acid is an H+ donor, and a Bronsted-Lowry base is an H+ acceptor and solvents besides water are envisioned. Finally, a Lewis acid is an electron acceptor, and a Lewis base is an electron donor, and acid base reactions that only satisfy Lewis' definition are explained. Also covered is how to identify conjugate acid-base pairs using the Bronsted-Lowry acid and base definitions. Finally, strong acids and bases are defined and a list of strong acids and a list of strong bases are provided.

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00:00 Lesson Introduction
00:26 Arrhenius Acids and Bases
03:31 Bronsted-Lowry Acids and Bases
06:50 Lewis Acid and Base
13:16 Conjugate Acid-Base Pairs
23:05 Strong Acids and Strong Bases

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