Colligative properties (5/11)

decrease the temperature at which the solution can freeze (must be even colder) and increase the temperature at which it boils (must get even hotter)

Do not depend on identity of solute Depend on the total number of dissolved solute particles

Vapor pressure reduction Boiling point elevation Freezing point depression Osmotic pressure

if liquid exposed to air will evaporate and this is the pressure if adding solute, reduced evaporation liquid pressure

Pvaporofsolution= Xmolefractionofsolvent*Pvaporof solvent Molefraction= mol of solvent/moles of solvent + moles of solute

temperature at which vapor pressure equals atmospheric pressure adding a solute to a solution decreases vapor pressure and increases boiling point

Tb = i*Kb*m Kb= constant for the solvent in question m= molality (mol/kg) i= how many particles generated when substance ionizes in solution

Tf=iKfm Kf water= 1.86 becomes less

Pressure required to prevent osmosis

adding a large amount of a nonvolatile solute to the solvent