Acids and Bases Glossary

Substance that donates protons (Bronsted-Lowry) or accepts electron pairs (Lewis).

Substance that accepts protons (Bronsted-Lowry) or donates electron pairs (Lewis).

Solution that resists changes in pH when small amounts of acid or base are added.

Acid-base pair differing by one proton: HA/A-.

Point in titration where moles of acid equal moles of base.

pH = pKa + log([A-]/[HA]) for buffer calculations.

Acid dissociation constant measuring strength of a weak acid.

Base dissociation constant measuring strength of a weak base.

Ion product of water: Kw = [H+][OH-] = 1.0e-14 at 25C.

Species that accepts an electron pair to form a coordinate bond.

Negative logarithm of hydrogen ion concentration: pH = -log[H+].

Negative logarithm of hydroxide concentration: pOH = -log[OH-]. pH + pOH = 14 at 25C.

Acid capable of donating more than one proton per molecule.