Solution - a homogeneous mixture of ions or molecules

Solute - the dissolved substance

Solvent - the dissolving medium

“Like dissolve like” principle - two substances with intermolecular forces of similar type and magnitude are likely to be soluble

Solubility - the amount of a substance that dissolves in a solvent

Saturated solution - one holding as much solute as is allowed at a stated temperature

Molarity - of a solute is the amount of moles that dissolves in a volume of the solution at a given temperature

Molality - the moles of solute per kilogram of solvent

Nonpolar solvents dissolve _ solutes - Nonpolar solvents dissolve NONPOLAR solutes

Polar solvents dissolve _ solutes - Polar solvents dissolve POLAR solutes

Similar intermolecular forces = _ - Solution

Different intermolecular forces = _ - No Solution

Henry’s Law - solubility of a gas in a liquid is proportional to partial pressure of the gas in contact with the liquid

∆H ion ion - Energies holding solute ions in crystal lattice

∆H dipole dipole - Energies holding solvent molecules together

∆H ion dipole - attractions between solute ions and solvent molecules

Lattice Energy [U] - The energy released when one mole of the ionic compound forms form its free ions in the gas phase

Colligative Properties - those properties that depend on solute concentration

4 Colligative properties of solutions - 1. vapor pressure reduction 2. freezing point depression 3. boiling point elevation 4. osmosis

Raoult’s Law - vapor pressure of a solution containing a solute is proportional to the mole fraction of the solvent

Boiling Point Elevation - Because vapor pressure is reduced in the presence of a nonvolatile solute a greater temperature must be reached to achieve boiling

Osmosis - movement of solvent through semi-permeable membrane from region of low solute concentration to region of higher solute concentration

Osmotic Pressure - pressure required to halt flow of solvent through membrane due to osmosis