1. Colligative Properties

2. Colligative Properties
~properties that depend only on the solute’s concentration rather than what the solute is
Simply adding a solute to a solvent will always have certain effects on the resulting solution.

3. Boiling point elevation/freezing point depression
All solutions will freeze at a lower temperature and boil at a higher temperature.
Boiling point elevation and freezing point depression are colligative properties.
That is to say it doesn’t matter what the solute dissolved in a solution, it will always boil at a higher temperature and freeze at a lower temperature.

4. Where it is used
Road salt goes into solution with snow, ice and water on the roads and lowers the freezing point.
Since it a colligative property, it doesn’t matter what the solute is. Just whatever is available in that area.
Water below the freezing point will not freeze and runs off the road, making it easier for a snow plow to clear the road.

5. Boiling Water
Students often assume that all boiling water is exactly at 100.0o C.
That is normally not the case because of two factors; the air pressure, and anything dissolved in the water.
Anything dissolved in the water will always raise the boiling point.

6. Calculations for boiling point elevation or freezing point depression
T = change in temperature
Boiling point elevation = BPnormal + T
Where T = Kb (m)i
Freezing Point Depression = FPnormal - T
Where T = Kf (m)i
Kb is the ebulliscopic constant
Kf is the cyroscopic constant
m is concentration of the solution in molality
i is the Van’t Hoff factor

7. Van’t Hoff Factor (i)
Colligative properties means it doesn’t matter what the solute is.
Some things when dissolved dissociate (ionic compounds), which, if you don’t care what the solute is technically would increase the molality.
NaCl (s) →Na+ (aq) + Cl- (aq)
Sodium chloride dissociates into 2 things
So it’s Van’t Hoff factor is 2
C6H12O6(s) → C6H12O6 (aq)
Glucose is a covalent compound that doesn’t dissociate, so it’s Van’t Hoff factor is 1

8. Freezing Point Depression and Boiling Point Elevation
Solvent
Formula
Melting Point (°C)
Boiling Point (°C)
Kf(°C/m)
Kb(°C/m)
Water
H2O
0.000
1.858
0.512
Acetic acid
HC2H3O2
16.60
118.5
3.90
3.08
Benzene
C6H6
5.455
80.2
5.12
2.53
Chloroform
CH2O
-63.5
61.3
4.68
3.63
Carbon disulfide
CS2
-112
46.3
3.8
2.34
Cyclohexane
C6H12
6.55
80.74
20.0
2.79
Ethanol
C2H5OH
-114.6
78.3
1.99
1.07

9. Problems We will only do a few problems with water solutions.
I will give you the Kf or Kb on the test. You are expected to know the normal boiling and melting point of water.

10. Freezing point problem
Determine the freezing point of a 2.1 m solution of water with calcium chloride (CaCl2) dissolved in it. Kf = °C/m
(Van’t Hoff) CaCl2 →Ca Cl- = 3
T = Kf (m)i
T = (2.1) 3= 4.1
FPwater = 0.00 – 2.6 = -4.1o C

11. Boiling point problem
Determine the freezing point of a 1.7 m solution of water with potassium nitrate (KNO3) dissolved in it. Kb = .512 °C/m
(Van’t Hoff) KNO3 →K+ + NO3- = 2
T = Kb (m) i
T = .512 (1.7) 2= 1.7
FPwater = = 101.7o C

12. Freezing point problem
Determine the freezing point of a 3.1 m solution of water with scandium bromide (ScBr3) dissolved in it. Kf = °C/m
(Van’t Hoff) ScBr3 →Sc Br- = 4
T = Kf (m) i
T = (3.1) 4= 23
FPwater = 0.00 – 2.6 = -23o C

13. Boiling point problem
Determine the freezing point of a 2.7 m solution of water with potassium sulfate (K2SO4) dissolved in it. Kb = .512 °C/m
(Van’t Hoff) KNO3 →2 K+ + SO42- = 3
T = Kb (m) i
T = .512 (2.7) 3= 4.1
FPwater = = o C

14. Vapor Pressure Vapor pressure lowering is a colligative property.
Vapor pressure, the amount of a liquid that will evaporate above a liquid, will be lower if anything is dissolved in it.
If you have a mixture of two volatile liquids the one with a higher normal vapor pressure will evaporate at a higher rate.

15. Fractional distallation
Fractional distillation makes use of vapor pressure lowering.
Fractional distillation is used to separate petroleum or crude oil.
Petroleum is a mixture of volatile liquids.
The vapors above will be much more pure than the solution because the most volatile will lower the amount of other substances that can evaporate

16. Fractional Distillation

17. Chromatography Separating a solution by capillary action
~the attraction of a liquid to the surface of a solid, why water “climbs up things”
For a simple chromatography place ink on chromatography paper and place the paper in a solvent with the ink above the water line.
The solvent will “climb up” and separate the ink

18. Chromatography
In chromatography, a mobile phase carries something through a stationary phase.
If different constituents have move at different speeds the material will be separated
In simple paper chromatography the water is the mobile phase, the paper is the stationary phase.

20. Other types of chromatography
Gas chromatography
TLC, thin layer chromatography
Column Chromatography
HPLC, high performance liquid chromatography

21. Homework Determine the boiling point of a 1.5 m solution Al(ClO3)3.
Determine the freezing point of a 2.9 m solution of Ca(MnO4)2.
Kf = °C/m
Kb = .512 °C/m