Chapter 11: Properties of Solutions

These flashcards cover key terms and definitions related to solution composition, colligative properties, and the behaviors of solutions in different contexts.

Solution

A homogeneous mixture formed when one or more substances are dissolved in another substance.

Molarity (M)

The number of moles of solute per liter of solution.

Mass percent

The mass of solute divided by the total mass of solution, multiplied by 100.

Mole fraction (x)

The ratio of the number of moles of a component to the total number of moles of all components in the solution.

Molality (m)

The number of moles of solute per kilogram of solvent.

Normality (N)

The number of equivalents of solute per liter of solution, often used in acid-base reactions.

Enthalpy of solution (ΔHsoln)

The heat change that occurs when a solute dissolves in a solvent.

Henry's Law

States that the concentration of a gas in a liquid is proportional to the partial pressure of the gas above the liquid.

Raoult’s Law

Describes how the vapor pressure of a solution is related to the vapor pressures of its components and their mole fractions.

Colligative properties

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

Boiling-point elevation

The increase in the boiling point of a solvent when a solute is dissolved, proportional to the molality of the solution.

Freezing-point depression

The decrease in the freezing point of a solvent when a solute is dissolved in it, also proportional to the molality.

Osmotic pressure (π)

The pressure required to stop osmosis, proportional to the molarity of the solution.

Ionic solute

A substance that dissociates into ions in solution, affecting colligative properties.

Electrolyte

A substance that dissociates into ions in solution, capable of conducting electricity.

Non-ideal solution

A solution that deviates from Raoult’s law due to strong interactions between solute and solvent.

Ideal solution

A solution that obeys Raoult’s law throughout all concentrations.

Tyndall effect

The scattering of light by particles in a colloid, used to distinguish colloids from true solutions.

Colloid

A mixture where small particles of one substance are dispersed within another substance.

Coagulation

The process by which colloidal particles clump together and settle out of suspension.

Hydrophilic

Substances that are attracted to water and can dissolve in it.

Hydrophobic

Substances that repel water and do not dissolve in it.