Acid-Base Equilibria
Chapter 14
Acid-Base Vocabulary
Arrhenius acid: proton donor
Arrhenius base: hydroxide donor
Bronsted-Lowry acid: proton donor
Bronsted-Lowry base: proton acceptor
Lewis acid: electron pair acceptor
Lewis base: electron pair donor
Polyprotic: having more than one available proton (acid group)
Amphiprotic: can act as either an acid or a base
Characteristics of Acids and Bases
Strong acid/base: completely dissociate in solution
Weak acid/base: partially dissociate in solution
Important Acid/Base Reactions
acid dissociation in water
base dissociation in water
strong acid-strong base neutralization
strong acid-weak base neutralization
weak acid-strong base neutralization
autoionization of water
Important Acid/Base Equations
How to find the Ka of an acid from pH (4:00)
Buffers are important for maintaining a constant pH in a solution. Titrations are a useful analytic tool that chemists use to determine the concentrations of unknown solutions. Click here to learn more about buffers and acid-base titrations.