Acid/Base Definitions

Arrhenius defintion

An Arrhenius acid increases the concentration of hydrogen ions (H+) in water, while an Arrhenius base increases the concentration of hydroxide ions (OH−).

Bronsted-Lowry definiton

defines acids as proton (H⁺) donors and bases as proton (H+) receivers (bases gain, acids lose)

Lewis Acid

electron acceptor: any molecule or ion that can accept a pair of nonbonding electrons. They are generally electron-deficient, such as compounds with less than an octet of electrons

Lewis base

electron donor: any molecule or ion that can donate a pair of nonbonding electrons. They are generally electron-rich, possessing lone pair electrons

How is Ka related to the strength of an acid?

acids with a higher Ka are stronger and have a lower pH

How are Ka and pKa related?

when Ka goes up pKa goes down, they are inversely related