Proton Transfer Reaction Flashcards
Bronsted-Lowry Theory
Acids are H+ donors
Bases are H+ accepters
Bronsted-Lowry Acid
Proton donor
Bronsted-Lowry Base
Proton Accepter
Conjugate Acid-Base Pair
A pair of species differing by a single proton
What must always be true when an acid donates a proton?
There must always also be a base present to accept the proton
Which Conjugate Acid-Base Pair is found in all aqueous acid-base reactions and how does it form?
H2O and H3O+
Forms when a proton is released from acid and associates with H2O molecules
Arrhenius Theory
Acids dissociate in water to produce H+ in solution
Bases dissociate in water to produce OH-in solution
Lewis Theory
Acids accept a pair of e- and bases donate a pair of e-
Strong acids
Equilibrium lies far to the right. Reactants are almost all dissociated (large K value). Strong acids yield weak conjugate bases
Weak acids
Equilibrium lies far to the left. reactants only dissociate to a small extent (small K value). Weak acids yield strong conjugate bases
Common strong acids
H2SO4
HNO3
HCl
HClO4
Common weak acids
H2CO3
H3PO4
HNO2
HClO
Organic acids
Contain carboxyl group-COOH
CH3COOH -Acetic Acid
C6H5COOH -Benzoic acid
Hydrohalic acids
Hydrogen with halogen, the stronger the bond between the hydrogen and halogen, the weaker the acid
HF - weak
HCl - strong
HBr - strong
HI - strong
Oxyacids
Oxygen attached to a central atom, the oxygen has a hydrogen attached to it. The more oxygen the stronger the acid
HClO4 - strong
HClO3
HClO2
HClO - weak
Strong bases
Equilibrium lies far to the right. Lots of OH-. The conjugate acid of a strong base is weak.
Group 1 + 2 with OH-
NaOH - strong
Ca(OH)2 - strong
Weak bases
Equilibrium lies far to the left. Reactants dissociate to a small extent. The conjugate acid of a weak base is strong
NH3
NH2 - amines
CH3NH2 - methylamine
C2H5NH2 - ethylamine
Hydroxides of metals that are not group 1 or 2 - Fe(OH)3
