"In chemistry, colligative properties are those properties of solutions that depend on the ratio of the number of solute particles to the number of solvent particles in a solution, and not on the nature of the chemical species present."
Physical properties of solutions that depend on the concentration of solute particles, but not on their identity. Examples include lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Solution: A homogeneous mixture of two or more substances.
Solvent: A substance that dissolves another substance to form a solution.
Solute: A substance that gets dissolved in a solvent.
Solubility: The ability of a substance to dissolve in a given solvent to form a solution.
Molarity: A measure of the concentration of a solution in terms of the number of moles of solute per liter of solution.
Molality: A measure of the concentration of a solution in terms of the number of moles of solute per kilogram of solvent.
Colligative properties: The physical properties of a solution that depend on the concentration of solute particles in the solution.
Raoult's law: A law that describes the vapor pressure lowering of a solvent in the presence of a nonvolatile solute.
Boiling point elevation: An increase in the boiling point of a solvent due to the addition of a solute.
Freezing point depression: A decrease in the freezing point of a solvent due to the addition of a solute.
Osmosis: The movement of solvent molecules from a region of low solute concentration to a region of high solute concentration through a semipermeable membrane.
Osmotic pressure: The pressure required to prevent the osmotic flow of solvent molecules across a semipermeable membrane.
Boiling point elevation: The boiling point of a solvent is raised when a non-volatile solute is added to it.
Freezing point depression: The freezing point of a solvent is lowered when a non-volatile solute is added to it.
Osmotic pressure: The pressure that must be applied to a solution to prevent the net flow of solvent through a semipermeable membrane from pure solvent to the solution.
Vapor pressure lowering: The vapor pressure of a solvent is lowered when a non-volatile solute is added to it.
Solubility: The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure.
Conductivity: The ability of a solution to conduct electricity due to the presence of ions in the solution.
Viscosity: The resistance of a fluid to flow.
Density: The amount of mass per unit volume.
Heat of Dilution: The enthalpy change that occurs when a solute is dissolved in a solvent.
Solubility product constant: The equilibrium constant of a sparingly soluble compound in a saturated solution.
"Colligative properties depend on the ratio of the number of solute particles to the number of solvent particles in a solution."
"The number ratio can be related to the various units for concentration of a solution such as molarity, molality, normality, etc."
"The assumption that solution properties are independent of the nature of solute particles is exact only for ideal solutions, which are solutions that exhibit thermodynamic properties analogous to those of an ideal gas, and is approximate for dilute real solutions."
"Colligative properties are a set of solution properties that can be reasonably approximated by the assumption that the solution is ideal."
"Only properties which result from the dissolution of a nonvolatile solute in a volatile liquid solvent are considered."
"All colligative properties have a common feature, namely that they are related only to the number of solute molecules relative to the number of solvent molecules and not to the nature of the solute."
"Colligative properties include: Relative lowering of vapor pressure (Raoult's law), Elevation of boiling point, Depression of freezing point, Osmotic pressure."
"For a given solute-solvent mass ratio, all colligative properties are inversely proportional to solute molar mass."
"Measurement of colligative properties for a dilute solution of a non-ionized solute such as urea or glucose in water or another solvent can lead to determinations of relative molar masses."
"Alternatively, measurements for ionized solutes can lead to an estimation of the percentage of dissociation taking place."
"Colligative properties are studied mostly for dilute solutions."
"Dilute solutions behave as that of an ideal solution."
"At higher concentrations, the freezing point depression, boiling point elevation, vapor pressure elevation or depression, and osmotic pressure are all dependent on the chemical nature of the solvent and the solute."