Tremendous amount of vocabulary here:
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Solutions
Solute
Solvent
Solution
Soluble
Insoluble
Miscible
Immiscible
Saturated
Unsaturated
Supersaturated
Solubility
Solutions are the physical mixture of two
substances. The substances can be in any
state.
Substances will mix when their polarities
are similar. “like dissolves like” is a good
rule-of-thumb.
Factors which affect Solubility:
 Temperature
o Ionic solids increase solubility
with increasing temperature
o Gases decrease solubility with
increasing temperature
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Pressure
o Does not effect solubility of
liquids and solids
o Gases increase solubility with
increased pressure (think can
of soda here): Directly
proportional
o Henry’s Law:
Sf
Pf

Si
Pi
Concentration:
 This is a very specific assignment of
how much solute is mixed with how
much solvent.
 Molarity (M):
o Remember, problems can
include mass instead of moles:
you will need to convert the
mass to moles first, and then
us it in the following:
Molarity( M ) 
moles of solute n

liters of solution V
Colligative Properties:
properties of a solution that depend only
on the amount of solute in the solution
 Vapor pressure lowering (VPL):
vapor pressure for a solution is
lower at a given temperature than
the vapor pressure of the pure
solvent
 Freezing point depression (FPD):
freezing point of a solution is
therefore lower than the freezing
point of the pure solvent

Boiling point elevation (BPE): boiling
point of a solution is therefore higher
than the boiling point of the pure
solvent
Test Reference: Holt Chemistry, Chapter
13
Practice Problems
1. Use the solubility graph on the preceding page to answer the following:
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What is the solubility of NaCl at 80 degrees Celcius?
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What substance is more soluble at 50 degrees: ammonia or potassium nitrate?
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How much HCl dissolves in 200 g H2O at 30 degrees Celcius?
2. Oxygen is much less soluble in water than carbon dioxide, 0.00412 g/100 mL at 20 °C
and 760 mm Hg. Calculate the solubility of oxygen gas in water at 20 °C and a
pressure of 1150 mm Hg.
3. What is the molarity when 0.75 mol is dissolved in 2.50 L of solution?
4. Suppose you had 58.44 grams of NaCl and you dissolved it in exactly 2.00 L of solution.
What would be the molarity of the solution?
5. Calculate the molarity of 25.0 grams of KBr dissolved in 750.0 mL.
6. Calculate the molarity when 75.0 grams of MgCl2 is dissolved in 500.0 mL of solution.
7. A solution of NaCl and water is made. What happens to the vapor pressure of the
solution compared to the pure solvent?