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Acids and Bases
Strong Bases: (all molecules deprotonate) Strong Acids: (all molecules deprotonate)
LiOH NaOH HCl HBr
KOH RbOH HI HNO3
CsOH HClO4 HClO3
Acid is a substance that yields H+ in solution
Base is a substance that yields OH-in a solution
Bronsted-Lowry Acid-Base Theory:
Acids are proton donors (Deprotonation)
Bases are proton acceptors
Bronsted-Lowry Acid is also a Lewis Acid, but a Lewis Acid is not necessarily a Bronsted-Lowry Acid because the Lewis definition is more general.
Determine which acids/oxides are strongest to weakest:
Look at # of O
Does it have 1 or 2 H’s or more?
K and Endo/Exo Reactions:
If Endothermic : K will increase if temperature increases and decrease if temperature decreases
If Exothermic: K will increase if temperature decreases and decrease if temperature increases
Kw= [H3O+] [OH-] Kw= 1.0 x 10-14
pX= -log[Xx] [Xx]=10-pX
Cation: Acid Anion: Base
pH= pKa + log (conj. Base/acid)