AP Chem Chapter 8

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.