Chem lecture 9

Arrhenius Acid

A substance that increases the concentration of hydrogen ions when dissolved in water.

Arrhenius Base

A substance that increases the concentration of hydroxide ions when dissolved in water.

Brønsted–Lowry Acid

A substance that donates protons (H+).

Brønsted–Lowry Base

A substance that accepts protons (H+).

Amphiprotic

A substance that can act as both an acid and a base.

Conjugate Acid–Base Pair

Two formulas that differ by H+, consisting of an acid and its corresponding base.

Autoionization of Water

The process where water acts as both an acid and a base resulting in the formation of H3O+ and OH-.

Kw

The ion product constant for water, which equals 1.0 × 10−14 at 25 °C.

Neutral Solution

A solution where [H+] = [OH-].

Acidic Solution

A solution where [H+] > [OH-].

Basic Solution

A solution where [H+] < [OH-].

pH Formula

pH = -log[H+].

pKw

The negative logarithm of the ion product constant for water, pKw = 14.00 at 25 °C.

Strong Acid

An acid that is 100% dissociated in water.

Weak Base

A base that has a low affinity for protons.

Proton Transfer Equilibrium

An equilibrium that favors the reaction of the stronger acid with the stronger base.