Acid and base definition

* Arrhenius
acid: generates [H+] in solution
base: generates [OH-] in solution
normal Arrhenius equation: acid + base <---> salt + water
example: HCl + NaOH <---> NaCl + H2O

* Bronsted-Lowery:
acid: anything that donates a [H+] (proton donor)
base: anything that accepts a [H+] (proton acceptor)
normal Bronsted-Lowery equation: acid + base <---> acid + base
example: HNO2 + H2O <---> NO2- + H3O+
Each acid has a conjugate base and each base has a conjugate acid. These
conjugate pairs only differ by a proton. In this example: HNO2 is the acid, H2O
is the base, NO2- is the conj. base, and H3O+ is the conj. acid.

* Lewis:
acid: accepts an electron pair
base: donates an electron pair
The advantage of this theory is that many more reactions can be considered
acid-base reactions because they do not have to occur in solution.