16.1 Introduction to Acids and Bases | General Chemistry

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.

Arrhenius Acids and Bases
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.

Bronsted Acids and Bases
A Bronsted-Lowry acid is an H+ donor, and a Bronsted-Lowry base is an H+ acceptor and solvents besides water are envisioned.

Lewis Acids and Bases
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.

Conjugate Acid-Base Pairs
Also covered is how to identify conjugate acid-base pairs using the Bronsted-Lowry acid and base definitions.

Strong Acids and Bases
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 (Bronsted Acids and Bases)
06:50 Lewis Acids and Bases
13:16 Conjugate Acid-Base Pairs
23:05 Strong Acids and Strong Bases

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