UNIT 7

Disassociation

The process by which an ionic compound separates into its constituent ions when dissolved in a solvent.

Ionization

The process by which a neutral atom or molecule gains or loses electrons to form ions.

Strong electrolyte

A substance that completely dissociates into ions in solution, conducting electricity effectively.

Weak electrolyte

A substance that only partially dissociates into ions in solution, conducting electricity weakly.

Net ionic equation

An equation that shows only the species that actually participate in the reaction, omitting spectator ions.

Molarity

A measurement of concentration, defined as the number of moles of solute per liter of solution.

Binary acids

Acids that consist of two elements, typically hydrogen and a nonmetal.

Oxyacids

Acids that contain hydrogen, oxygen, and another element (the central atom, often a nonmetal).

Arrhenius definition of acid

An acid is a substance that increases the concentration of hydrogen ions (H⁺) in aqueous solution.

Arrhenius definition of base

A base is a substance that increases the concentration of hydroxide ions (OH⁻) in aqueous solution.

Bronsted-Lowry definition of acid

An acid is a proton donor.

Bronsted-Lowry definition of base

A base is a proton acceptor.

Conjugate acid

The species formed when a base gains a proton.

Conjugate base

The species that remains after an acid has donated a proton.

pH scale

A logarithmic scale used to specify the acidity or basicity of an aqueous solution.

pOH

A measure of hydroxide ion concentration in a solution, related to pH as pH + pOH = 14.

Titration

A laboratory method used to determine the concentration of a solution by reacting it with a standard solution.

Equivalence point

The point in a titration at which the added titrant is stoichiometrically equivalent to the substance being titrated.