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As temperature increases, solubility ______ for solids but _______ for gas.
A colligative property is a physical property that is dependent on ________ ?
The # of solute particles but not their identity
As # of particles increases, vapor pressure ______.
As # of particles increases, freezing point _______.
As # of particles increases, boiling point ______.
Vapor Pressure ________
Boiling Point _______
Freezing Point _______
What is the van't Hoff factor?
i = the # of particles the substance breaks into
As # of particles increase, osmosis pressure _______.
How many particles does 2m NaCl have?
- NaCl -> Na + Cl
- 2 particles X 2m = 4
How many particles does 2m CH3COOH have?
- Weak electrolyte so partially dissociates into ions.
- 1 < i < 2
- 2-4 particles
All non-electrolytes have what van't Hoff factor?
i = 1
In an equation, use the van't Hoff factor for the ______ & the constant for the ________.
In an equation, when do u worry about the van't Hoff factor?
When the solute is a strong or weak electrolyte
How do u find the change in temperature of boiling point?
Constant of solvent X van't Hoff factor (if necessary) X molality
After finding the change of boiling temp, how do u find the temperature of the solution?
- Take ur change in temp & add it to the boiling of solvent (in celsius)
- E.G. Change in temp is .34 so add that to 100 (water's boiling point) = 100.34 C
How do u find the temperature change in freezing point?
Constant of freezing solvent X van't Hoff factor (if necessary) X molality
After finding the change in freezing temp, how do u find the freezing point for the solution?
- Subtract the change in freezing temp from the freezing point of the solvent.
- E.G. Change in temp is 1.23 so subtract that from 0 (water's freezing point) =
- -1.23 C
What is Raoult's Law? (Vapor Pressure)
- Pa = Xa (Pure a)
- Solution's vapor pressure = mole fraction X pure solvent's vapor pressure
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