1. Colligative Properties of Solutions
Reaction Rates…
How can I make a reaction happen faster?

2. What is a colligative property?
A property that depends on:
the concentration of solute particles in solution
the solvent used
A colligative property does not depend on:
1. the identity of the solute

3. Dilute Versus Concentrated Solutions
Dilute--> a low amount of solute is dissolved in a solvent
Concentrated--> a high amount of solute is dissolved in a solvent
These terms will not tell us whether a solution is saturated, unsaturated, or supersaturated
The concentration of a solution can be found using the Molarity (M) and Molality (m) equations

4. Freezing Point Depression
When a solute is dissolved in a solvent, the freezing point of the solvent will depress (become lower) than the normal freezing point of the pure solute

5. What does the FP depression depend on?
The amount the FP will be lowered depends on 3 factors:
The concentration of the solution
Higher molality (m) = higher depression
Whether or not the solution is an electrolyte
Electrolytes = higher depression
The identity of the solvent used
H2O vs. C2H5OH will exhibit different depressions

6. What is an electrolyte?
A substance that MUST contain ions and conducts electricity (metal & nonmetal)
Electrolytes break apart into + and - charged particles which would have a greater effect on the FP depression

7. Which of the following are examples of electrolytes?
NaCl, C12H22O11, CaCl2, C2H5OH
How many ions do each of the electrolytes have?

8. How do you find the FP depression of the solvent?
∆Tf = kf n m
∆Tf = FP depression (how many °C lower than the FP of the pure solvent)
Kf = FP constant which is dependant on the solvent used (table provided on next slide)
n = number of ions (if applicable)
m = molality of the solution

10. Sample Problem #1
How much will the freezing point be lowered if enough sucrose (C12H22O11) is dissolved in H2O to make a .50 m solution?
What if the solute was barium bromide? Calculate the FP depression.

11. Sample Problem #2
What is the freezing point depression of a solution containing 16.5 g of sodium chloride in 300. g of acetic acid?
What is the freezing point of the solution?

12. Sample Problem #3
What is the concentration of a nonelectrolyte tincture that has a depression of 2.8°C. Methanol is the solvent used to make this tincture.
What is the freezing point of the tincture?

13. Practical Application of FP Depression
Why does putting salt on the roads when it is icy prevent the roads from being slick?
The addition of salt as a solute will lower the FP of H2O and help to prevent ice from forming

14. Boiling Point Elevation
When a solute is dissolved in a solvent, the boiling point of the solvent will elevate (become higher) than the normal boiling point of the pure solute
BP elevation depends on the same factors that FP depression does

15. How do you find the BP elevation of the solvent?
∆Tb = kb n m
∆Tb = BP elevation (how many °C higher than the BP of the pure solvent)
Kb = BP constant which is dependant on the solvent used (table)
n = number of ions (if applicable)
m = molality of the solution

16. Sample Problem #1
What is the boiling point elevation of a 1.3 m solution of sucrose dissolved in ethanol?
What is the boiling point of the solution?

17. Sample Problem #2
What is the expected boiling point elevation of an aqueous solution that contains 136 g of potassium nitrate in 1.00 kg?
What is the boiling point of the solution?

18. Sample Problem #3
A nonelectrolyte solute is dissolved in 50 kg of benzene (C6H6). The new BP of this solution is 80.61ºC. What is the amount in moles of solute if pure benzene boils at 80.10ºC?

19. Practical Application of BP Elevation
Why do cooks add salt to their water when boiling water?
The addition of salt as a solute will force the H2O to boil at a higher temperature which will in turn, cook the food placed in the H2O faster

20. What Factors Affect the Rate of a Reaction?
1. Increase in surface area
Ex. Increasing the surface area of a substance allows for more particle contact and collisions, therefore increasing the rate of a reaction
Granulated sugar should dissolve more quickly in a solvent because of its greater surface area

21. 2. Increase in temperature
Ex. Increasing the temperature of a reaction allows for more frequent particle contact and collisions due to an increase in the kinetic energy of the system, therefore increasing the rate of a reaction

22. 3. Increase in concentration of reactants
Ex. Increasing the concentration of reactants allows for more particle collisions because there are more particles present, therefore increasing the rate of a reaction

23. 4. Addition of a catalyst
Ex. The addition of a catalyst will force the particles to come in contact at a quicker rate, therefore increasing the rate of the reaction
• 5. Agitation/Stirring

24. The Collision Theory
In order for a reaction to occur, 2 particles must have an effective collision. A successful collision needs:
1. Proper orientation (particles must hit in the right spots)
2. Suitable kinetic energy (particles must hit with the right amount of speed --> too much or too little may result in an ineffective collision)

26. Reaction Rate Diagrams
Activation Energy (Ea) = the energy needed to get a reaction started
This diagram is representing an exothermic reaction because energy is being released and the products contain less energy than the reactants
Lowers Ea

27. Inhibitors increase Ea by slowing down a reaction