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Bronsted-Lowry Acid
A substance that donates protons (H+ ions) in a chemical reaction.
Bronsted-Lowry Base
A substance that accepts protons (H+ ions) in a chemical reaction.
Arrhenius Acid
A substance that produces H3O+ ions when dissolved in water.
Arrhenius Base
A substance that produces OH- ions when dissolved in water.
Kw
The equilibrium constant for the autoionization of water, equal to 1×10^-14 at 298K.
pKw
The negative logarithm of the ionic product of water, which equals 14 at 298K.
Equilibrium constant equation
pKw = pKa + pKb.
Strong Acid + Strong Base
Results in a pH determined by the excess reagent.
Weak Acid + Strong Base
Buffering occurs if the weak acid is in excess; pH is influenced by excess OH- if the strong base is excess.
Weak Base + Strong Acid
Buffering occurs if the weak base is in excess; pH is influenced by excess H3O+ if the strong acid is excess.
Weak Acid + Weak Base
Reaches an equilibrium state.
Note 
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