Post on 12-Jan-2017
transcript
Colligative PropertiesPt. 3
By Shawn P. Shields, Ph.D.
This work is licensed by Shawn P. Shields-Maxwell under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License.
Colligative Properties
A physical property of a solution that depends only on the ratio of the number of particles of solute to solvent in the solution, not the identity of the solute.
Describes a nonvolatile solute dissolved in a solvent.
Four Colligative Properties
Boiling point elevation
Freezing point depression
Vapor pressure lowering
Osmotic pressure
How can we explain these?
Recall: Pressure-Temperature Phase Diagrams
PT
TT
1 atm
vapor
liquidsolid
triple point
X mp X bp
T (C)
P (atm)
Effect of Colligative Properties on the Phase Diagram
T (C)
P (atm)1 atm
Dotted lines indicate the new phase boundaries for the solution.
The solid-liquid coexistence line is now shifted to lower temperatures.
The liquid-vapor line shifts to higher temperatures.
Effect of Colligative Properties on the Phase Diagram
T (C)
P (atm)1 atm
new mpX
new bpX
Boiling point elevation
Melting point depression
Vapor pressure lowering (come back to this)
Boiling Point ElevationRecall: The boiling point of a substance is the temperature where the vapor pressure equals the external (usually atmospheric) pressure.
The external pressure doesnโt change, but the temperature required to attain that vapor pressure is increased!
Tb = kbmTb is the increase in boiling temperaturekbis the molal boiling point elevation constant (look it up for a given solvent)m is the molality of the solute
molality= moles solutekg of solvent
Freezing Point DepressionWhen the freezing point is depressed, this means the temperature must be lower before a given substance freezes.
Tf = kfm
Tf is the decrease in freezing temperaturekfis the molal freezing point depression constant (look it up for a given solvent)m is the molality of the solutemolality (m)=
moles solutekg of solvent
Calculating Solvent Mass
Use the volume of the solvent and its density to find the mass of solvent for molality (m).
๐ฆ๐จ๐ฅ๐๐ฅ๐ข๐ญ๐ฒ (๐ฆ)=๐ฆ๐จ๐ฅ๐๐ฌ๐ฌ๐จ๐ฅ๐ฎ๐ญ๐๐ค๐ ๐จ๐ ๐ฌ๐จ๐ฅ๐ฏ๐๐ง๐ญ
๐๐๐ง๐ฌ๐ข๐ญ๐ฒ ( ๐ ๐ฆ๐ )= ๐ฆ๐๐ฌ๐ฌ
๐ฏ๐จ๐ฅ๐ฎ๐ฆ๐
Recall: Equilibrium Vapor Pressure
Molecules in the liquid phase continuously vaporize and condense in a closed container.rate of evaporation = rate of condensation
The partial pressure of the gas is constant at equilibrium.
Liquid molecule
Vapor Pressure Lowering
The vapor pressure of the solution is lower than the pure solvent.
T (C)
P (atm)1 atm
Normal bp of pure solvent
VP at bp of pure solvent
X VP of solution
Raoultโs LawThe vapor pressure of the solution depends on the mole fraction of the solvent.
is the vapor pressure of the solution
is the mole fraction of the solvent
is the vapor pressure of the pure solvent
Raoultโs Law
The vapor pressure of the solution depends on the mole fraction of the solvent.
Liquid moleculeNonvolatile solute
Osmosis
The two regions are separated by a semipermeable membrane that allows solvent to pass, but not solute particles.
Osmosis By OpenStax College [CC BY 3.0 (http://creativecommons.org/licenses/by/3.0)], via Wikimedia Commons
The net movement of solvent molecules from a region of lower solute concentration to one with a higher concentration.
Osmotic Pressure ()Osmotic pressure is the amount of pressure required to stop the flow of solvent. A similar equation to the Ideal Gas law can be written for the osmotic pressure:
Where is the osmotic pressure (in the same units as the gas constant, R)V is the volume in L, n is moles of solute, and T is temperature in K
Osmotic Pressure ()
We can rearrange this equation to a more useful form
Where C is the concentration (M, molarity)
Example Problemswill be posted separately.