Chemistry: Chapter 14: Mixtures and Solutions

suspension

a type of heterogeneous mixture whose particles settle out over time and can be separated from the mixture by filtration

colloid

a heterogeneous mixture of intermediate-sized particles (between atomic-size of solution particles and the size of suspension particles)

Brownian motion

the erratic, random, movements of colloid particles that results from collisions of particles of the dispersion medium with dispersed particles

Tyndall effect

the scattering of light by colloidal particles

soluble

describes a substance that can be dissolved in a given solvent

miscible

describes two liquids that are soluble in each other

insoluble

describes a substance that cannot be dissolved in a given solvent

immiscible

describes two liquids that can be mixed together but separate shortly after you cease mixing them

concentration

a measure of how much solute is dissolved in a specific amount of solvent or solution

molarity

the number of moles of solute dissolved per liter of solution; also known as molar concentration

molality

the ratio of the number of moles of solute dissolved in one kilogram of solvent; also known as molal concentration

mole fraction

the ratio of the number of moles of solute in solution to the total number of moles of solute and solvent

solvation

the process of surrounding solute particles with solvent particles to form a solution; occurs only where and when the solute and solvent particles come in contact with each other

heat of solution

the overall energy change that occurs during the solution formation process

unsaturated solution

contains less dissolved solute for a given temperature and pressure than a saturated solution; has further capacity to hold more solute

saturated solution

contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure

supersaturated solution

contains more dissolved solute than a saturated solution at the same temperature

Henry's law

states that at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid

colligative property

a property of a solution that depends on the number, not the identity, of the solute particles.

vapor pressure lowering

the lowering of the vapor pressure of a solvent caused by the presence of dissolved solute particles.

boiling point elevation

the temperature difference between a solution's boiling point and a pure solvent's boiling point.

freezing point depression

the difference in temperature between a solution's freezing point and the freezing point of its pure solvent.

osmosis

diffusion of a solvent through a semipermeable membrane.

Diffusion of water across a selectively permeable membrane

osmotic pressure

the amount of additional pressure caused by the water molecules that moved into the concentrated solution.

Solute

Solvent

Homogeneous mixture

Heterogeneous mixture