1. Henry’s Law, Freezing Point Depression, Boiling Point Elevation and Raoult’s Law
Wow, That is a Mouthful

2. Henry’s Law
The solubility of a gas is directly proportional to the gas pressure
Sg= khPg
When the partial pressure of the solute above a solution drops, the solubility of the gas in the solution drops as well to maintain the equilibrium.
This can be used to calculate the molar solubility of a gas.
What is the concentration of O2 in a fresh water stream in equilibrium with air at 25oC and 1.0 atm. (Hint there is 21% O2 in the air)

3. Does this always fit?
As concentrations and partial pressures increase, deviations from Henry's law become noticeable. This behavior is very similar to the behavior of gases, which are found to deviate from the ideal gas law as pressures increase and temperatures decrease. For this reason, solutions which are found to obey Henry's law are sometimes called ideal dilute solutions

4. Colligative Properties
Colligative properties are “properties that depend only on the relative number of particles and not on what the actual substance is”
Remember that

5. Changing Vapor Pressure (Raoult’s Law)
Vapor pressure at a given temperature is the pressure that the vapor exerts when the rate of molecules leaving the surface is equal to the rate of them re-condensing.
But what happens when something is now dissolved in the solvent.
2 things- 1. less solvent molecules at the surface. 2. different sets of attractive forces

6. Lets look at each one individually
1. less solvent molecules at the surface. Therefore less chance the water leaves, the vapor pressure is lowered.
This makes sense based on Henry’s law. The vapor pressure of the solvent will be proportional to the mole fraction in the liquid.
Psolvent= XsolventK
If we also look at a pure solvent Po,
then Po= XsolventK, Therefore Psolvent= Xsolvent Po
This is Raoult’s Law

7. Raoult’s Law
Raoult’s law assumes that the solution is ideal. Therefore, the forces between solute and solvent molecules must be the same as the solvent to solvent.
If solvent-solute interactions are stronger than solvent-solvent, the actual vapor pressure will be lower than calculated
If solvent-solute interactions are weaker than solvent-solvent, the actual vapor pressure will be higher than calculated

8. Try a problem
Assume you dissolve 10.0g of sugar (C12H22O11) in 225mL (225g) of water and warm the water to 60oC. What is the vapor pressure of the water over this solution? The normal vapor pressure of water at 60oC is torr.

9. Raoult’s Law Cont.
Adding a nonvolatile solute to a solvent will lower the vapor pressure.
∆Psolvent= Psolvent- Posolvent
∆Psolvent= (XsolventPosolvent) – Posolvent = -(1-Xsolvent)Posolvent
Xsolvent+Xsolute = 1
∆Psolvent= -XsolutePosolvent

10. Why does this matter?
Well remember that vapor pressure determines the boiling point of a liquid.
If you add solute it will change the solvent’s vapor pressure, therefore the boiling point changes.
This is called boiling point elevation!

11. Boiling Point Elevation
The Boiling point elevation, Δtbp, is directly proportional to the molality of the solute
Δtbp= Kbpmsolute
Kbp is called the molal boiling point elevation constant by solvent and is (oC/m)
How many grams of ethylene glycol, HOCH2CH2OH, do you have to add to 125 g of water to increase the bp by 1oC? (The KbpWater = oC/m

12. What is another use? Molar mass by boiling point elevation!
A solution prepared from 1.25 g of oil of wintergreen (methyl salicylate) in 99.0 g of benzene has a boiling point of 80.31oC. Determine the molar mass of the compound. (Benzene’s normal bp is and the Kbp is oC/m)
Answer is 150 g/mol

13. Freezing Point Depression
Very similar to boiling point
Δtfp= Kfpmsolute
The reason for this is very similar in changes in vapor pressure equilibrium
There are more atoms of pure solvent going from solid to liquid than from liquid to solid.

14. What about for electrolytes?
We would assume that adding NaCl or such to water would have twice the effect
That is pretty much true.
To see the real effect, we need a van’t Hoff factor
i = Δtfp, measured/ Δtfp calculated
As the Δtfp calculated is if no ionization occurred. The i is not a perfect for the number of ions, but is closest to it for dilute solutions due to the intermolecular attractive forces.
Δtfp, measured= Kfpmsolute i

15. Calculate the freezing point of 525 g of water that contains 25
Calculate the freezing point of 525 g of water that contains 25.0 g of NaCl. Assume i is 1.85 for NaCl.