What Ka Represents
Acid Dissociation Constant (only for weak acids); greater Ka = stronger acid
What Kb Represents
Base Dissociation Constant (only for weak bases); greater Kb = stronger base
What Kw represents
Water Dissociation Constant; [H⁺][OH⁻] = 10⁻¹⁴
Relationship between Conjugate Acids and Bases
Ka * Kb = Kw
What Ksp Represents
Solubility Product; greater Ksp = more soluble
What Q Represents
Reaction Quotient; if Q > k reactions is forward and vice versa
Le Châtelier’s Principle
If a system at equilibrium is disturbed
Henderson-Hasselbalch Equation
pH = pKa + log([Base]/[Acid])
Brønsted-Lowry acid
Proton (H⁺) donor
Brønsted-Lowry base
Proton (H⁺) acceptor
Arrhenius acid
Produces H⁺ in water
Arrhenius base
Produces OH⁻ in water
How to Determine Strong Acids
Hydrogen + Halogen (not F) OR # Oxygen - # Hydrogen >= 2
How to Determine Strong Bases
Group I
Strength of Nitrogen-Containing Bases
Weak
Strength of Carboxylic Acids
Weak
Homogeneous Catalyst
Catalyst in the same phase as the reactants
Heterogeneous Catalyst
Catalyst in a different phase than the reactants
