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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
Henrys 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
vapor pressure reduction 2. freezing point depression 3. boiling point elevation 4. osmosis
Raoults 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