chapter_12_powerpoint_l

Solution

A homogeneous mixture of two or more substances.

Solute

The substance(s) present in the smaller amount(s) in a solution.

Solvent

The substance present in the larger amount in a solution.

Saturated Solution

A solution that contains the maximum amount of solute that will dissolve at a specific temperature.

Unsaturated Solution

A solution that contains less solute than the solvent has the capacity to dissolve at a specific temperature.

Supersaturated Solution

A solution that contains more solute than is present in a saturated solution at a specific temperature.

Solvation

The process in which the particles of a solute are surrounded by solvent molecules.

Miscible

Two liquids that are soluble in each other in all proportions.

Colligative Properties

Properties that depend only on the number of solute particles in solution and not on the nature of the solute.

Vapor-Pressure Lowering

A colligative property described by Raoult's law, demonstrating how the vapor pressure of a solvent decreases in the presence of a solute.

Boiling-Point Elevation

An increase in the boiling point of a solvent when a solute is dissolved in it.

Freezing-Point Depression

A decrease in the freezing point of a solvent when a solute is added.

Osmotic Pressure

The pressure required to stop the passage of solvent through a semipermeable membrane in osmosis.

Henry’s Law

States that the solubility of a gas in a liquid is proportional to the pressure of the gas above the solution.

Fractional Crystallization

The separation of a mixture of substances into pure components based on their differing solubilities.

Ideal Solution

A solution that follows Raoult’s law throughout the entire range of concentrations.

Molality (m)

The number of moles of solute per kilogram of solvent.

Molarity (M)

The number of moles of solute per liter of solution.

Van't Hoff Factor (i)

The number of particles a compound dissociates into in solution.