Bronsted Lowry Acid/Base theory:
acid = proton (H+) donor
base = proton (H+) acceptor
Conjugate acids and bases differ only by 1 H+!
If an acid or base is…Then its conjugate base or acid is…
Strong Inert
Weak Weak
Strong Acids =pH Inert Anions Strong Bases = pH Inert Cations
HClCl- I II I II
HBrBr- LiOHLi+
HII- NaOHNa+
HNO-+2+3NO3 KOHCa(OH)2K Ca
HSOSO2-+2+244 RbOHSr(OH)2Rb Sr
CsOHBa(OH)Cs+ Ba2+2
Equations that will always be applicable:
[H+][OH-] = 1x10-14 pH = -log[H+]pOH = -log[OH-]
pH + pOH = 14
Remember that we take H+ and H+3O to synonymous.
