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The Colligative Properties definitions

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  • Colligative Properties
    Characteristics of solutions that depend on the number of dissolved particles, not their identity, affecting boiling, freezing, vapor pressure, and osmosis.
  • Boiling Point
    Temperature where liquid and gas phases reach equilibrium, with vaporization and condensation occurring at equal rates.
  • Freezing Point
    Temperature where solid and liquid phases are in equilibrium, with melting and freezing processes balanced.
  • Vapor Pressure
    Pressure exerted by a gas at the surface of a liquid when the system is at equilibrium.
  • Osmotic Pressure
    Force driving water movement across a membrane from low to high solute concentration, influencing solution levels.
  • Van't Hoff Factor
    Number representing country of ions produced when a soluble solute dissolves, impacting colligative effects.
  • Ionic Compound
    Substance composed of positive and negative ions, dissociating into multiple particles in solution.
  • Covalent Compound
    Molecule formed from nonmetals, remaining intact in solution without forming ions.
  • Nonvolatile Solute
    Substance that does not readily vaporize, remaining in the liquid phase and not contributing to vapor pressure.
  • Non-electrolyte
    Substance that does not produce ions in solution, thus not conducting electricity.
  • Osmolarity
    Total ionic concentration of a solution, calculated as the van't Hoff factor multiplied by molarity.
  • Osmolality
    Total ionic concentration per kilogram of solvent, found by multiplying the van't Hoff factor by molality.
  • Solution
    Homogeneous mixture formed when a solute is dissolved in a solvent, exhibiting altered physical properties.
  • Solvent
    Component present in greater amount in a solution, dissolving the solute and determining the phase.
  • Solute
    Substance dissolved in a solvent, altering the physical properties of the resulting solution.