8.A Acid–Base Equilibria

8.A.1 Brønsted–Lowry definition of acids and bases

“We see all those signs around acids… acid is dangerous Jeremy, but why?”

“They are highly corrosive, Miley.”

There are 3 definitions of an acid, in order of the date of creation:

1. Arrhenius, which defines an acid as anything that produces H+ (hydrogen) ions in aqueous solution.

2. Bronsted-Lowry

3. Lewis

8.A.2 Ionization of water

8.A.2.a Kw, its approximate value (Kw = [H3O+][OH–] = 10–14 at 25°C)

8.A.2.b pH definition, pH of pure water

More info: http://www.johnkyrk.com/pH.html

8.A.3 Conjugate acids and bases

8.A.4 Strong acids and bases (common examples; e.g., nitric, sulfuric)

8.A.5 Weak acids and bases (common examples; e.g., acetic, benzoic)

8.A.5.a dissociation of weak acids and bases with or without added salt

8.A.5.b hydrolysis of salts of weak acids or bases

8.A.5.c calculation of pH of solutions of weak acids or bases

8.A.6 Equilibrium constants Ka and Kb (pKa and pKb)

8.A.7 Buffers

8.A.7.a definition, concepts (common buffer systems)

8.A.7.b influence on titration curves

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