Acids, Bases, and Salts

Neutralization reaction

A reaction between an acid and a base that produces a salt and water.

Acidic solution

Any solution where the hydrogen ion concentration is greater than the hydroxide ion concentration.

Basic solution

Any solution where the hydrogen ion concentration is less than the hydroxide ion concentration.

Buffer

A solution of a weak acid or weak base and one of its salts that resists pH change.

Salt hydrolysis (Acidic)

Salts where positive ions release protons to water.

Salt hydrolysis (Basic)

Salts where negative ions attract protons from water.

Amphoteric

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

Indicator

A substance whose acidic and basic forms have different colors in solution.

Endpoint of titration

The point of neutralization where an indicator changes color.

Arrhenius Acid

A substance that yields hydrogen ions in aqueous solution.

Arrhenius Base

A substance that yields hydroxide ions in aqueous solution.

Bronsted-Lowry Acid

A hydrogen ion donor.

Bronsted-Lowry Base

A hydrogen ion acceptor.

Lewis Acid

A substance that can accept a pair of electrons to form a covalent bond.

Lewis Base

A substance that can donate a pair of electrons to form a covalent bond.

Strong Acid

An acid that completely ionizes in aqueous solution.

Weak Acid

An acid that only slightly ionizes in aqueous solution.

Monoprotic Acid

An acid containing one ionizable hydrogen, such as nitric acid.

Diprotic Acid

An acid containing two ionizable hydrogens, such as sulfuric acid.

Triprotic Acid

An acid containing three ionizable hydrogens, such as phosphoric acid.

Conjugate acid

The particle formed when a base gains a hydrogen ion.

Conjugate base

The particle that remains after an acid has donated a hydrogen ion.

Conjugate acid-base pair

Two substances related to each other by the gain or loss of a single hydrogen ion.

Self-ionization of water

The reaction where water molecules collide and produce ions.

Neutral solution (concentration)

A solution where the concentrations of hydrogen and hydroxide ions are equal.

Ion-product constant (Kw)

The product of the concentrations of hydrogen and hydroxide ions in water, equal to 1.0 times 10 to the power of negative 14.

pH

The negative logarithm of the hydrogen-ion concentration.

pOH

The negative logarithm of the hydroxide-ion concentration.

Acidic pH

A pH value less than 7.0.

Neutral pH

A pH value equal to 7.0.

Basic pH

A pH value greater than 7.0.

Neutralization

Acid plus Base produces Salt plus Water.

Water Constant

Hydrogen ion concentration times Hydroxide ion concentration equals 1.0 times 10 to the power of negative 14.

pH and pOH

pH plus pOH equals 14.