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-Physical properties of a solution differ from those of the pure solvent used to make the solution

This article explains the difference between the physical properties of a solution and those of the pure solvent it is made from. It also explores colligative properties, which depend only on the number of particles dissolved in a given mass of solvent. Topics covered include vapor pressure, boiling point elevation, freezing point depression, and the effects of solute particles on these properties.

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-Physical properties of a solution differ from those of the pure solvent used to make the solution

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  1. -Physical properties of a solution differ from those of the pure solvent used to make the solution colligative properties- depend only on the # of particles dissolved in a given mass of solvent • vapor pressure -pressure above the surface of a liquid -looking at non-volatile liquids (do not vaporize easily)

  2. -the solute decreases the vapor pressure because: -solute is surrounded by solvent in solvation process and less solvent molecules can escape -degree of dec. depends on # of particles of solute -ionic compounds cause more a dec. b/c they separate into their ions -molecular cause less of a dec. b/c they do not ionize (always 1 particle)

  3. ex- NaCℓ produces 2 particles sugar C12H22O11 produces 1 *polyatomic ions count as 1 unless ( ) Try These! How many particles when placed in solution? a) CaCℓ2 b) MgSO4 a) 3 b) 2 c) C2N2 d) Aℓ2(SO4)3 c) 1 d) 5

  4. boiling point -temp at which the vapor pressure equals the atmospheric pressure -increased when solute is added -degree of inc. depends on # of particles boiling point elevation- difference in temp between the boiling point of a solution and that of a pure solvent

  5. freezing point -temp at which liquid goes to solid -decreased when solute is added -degree of dec. depends on # of particles freezing point depression- difference in temp between the freezing point of a solution and that of a pure solvent

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