Acid Base Theory

1. Arrhenius Theory
Acid: electrolyte substance which in water produce H⁺ ion.
Example: HBr_(aq) → H⁺_(aq) + Br^-_(aq).
Base: electrolyte substance which in water produces OH-.
Example: KOH_(aq) → K⁺_(aq) + OH^-_(aq).


2. Bronsted Lowry Theory
Acid: substance that gives proton or H^+.
Base: oxygen proton or accept a H⁺.
Example: H₂O + NH₃ → NH₄⁺ + OH^-
acid1 basa1 acid2 base2
Base acid conjugation couple has characteristics deviate only 1 H⁺.
For the reaction on the spouse: H₂O and OH^-, NH₃ and NH₄⁺.
Substance amphipirotic/amfoter: substances that can give or receive
the proton (H⁺). Ex: H₂O, H₂PO₄^-,HPO₄^2-.


3. Lewis Theory

Acid: electron pair acceptor.
Base: electron pair donor.
Example: BF₃ + :NH₃ → H₃N:BF₃
NH₃ to give a pair of electrons to BF₃, NH₃ as base and BF₃ as acid.