Boiling temperature elevation- property of solutions that describes temperature difference between boiling point of a pure solvent and temperature at which solution begins to boil.
Colligative property- characteristic of a solution that does not depend on size or type of particles present as a solute but only on concentration of the particles, e.g., boiling point elevation and freezing point depression.
Dissociation- separation of a molecule into two or more fragments. Producing no new substances.
Electrolyte- separation of a molecule into two or fragments, producing no new substances.
Freezing point depression- property of solution that describes the temperature difference between the freezing point of a pure solvent and temperature at which a solution begins to freeze.
Heterogeneous mixture - mixture in which the parts are still visible.
Homogenous mixture- one in which the components are uniformly mixed and cannot be visually distinguished.
Hydrated- condition in which a charged ion is surrounded by water molecules.
Immiscible- not capable of being mixed.
Ionic equation- representation listing reactants and products as hydrated ions rather than in molecular form.
Molality- number of moles of solute per kilogram of solvent.
Net ionic equation- ionic equation without representation of spectator ions.
Precipitate- insoluble substance formed through a chemical reaction in a solution.
Saturated- condition that exists when a solution cannot dissolve any more solute at a given temperature.
Solubility- maximum quantity of a substance that will dissolve in a solvent.
Solute- component of a solution in the lesser amount.
Solution- mixture that looks uniform through out and does not scatter light.
Solvation- process of dissolving a solute in a solvent.
Solvent- component of a solution that is in the greater quantity.
Spectator ion- ion that is present but does not partic
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