1. Some Definitions
A solution is a _______________ mixture of 2 or more substances that appear uniform.
One part is regarded as the SOLVENT and the others as SOLUTES.

2. Solubility
the amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution
influenced by:
Pressure
Temperature
Solids increased temperature causes
them to be more soluble and vice versa
Gases increased temperature causes
them to be less soluble and vice versa
Ex. Iced Coffee
Solids increased pressure has no
effect on solubility
Gases increased pressure causes them
to be more soluble and vice versa
Ex. Soda, “The Bends”

3. Saturated v.s. unsaturated.
Solutions can be classified as saturated or unsaturated.
A saturated solution contains the maximum quantity of solute that dissolves at that temperature.
An unsaturated solution contains less than the maximum amount of solute that can dissolve at that temperature.

5. SUPERSATURATED SOLUTIONS
SUPERSATURATED SOLUTIONS contain more solute than is possible to be dissolved
Supersaturated solutions are unstable. The supersaturation is only temporary.
How can we make a supersaturated Solution?

6. Concentration of Solute
The amount of solute in a solution is given by its concentration.
Concentration is measured by a quantity called Molarity.
Molarity ( M ) =
moles solute
liters of solution

7. Finding Molarity
Calculate the molarity of a HCl solution if 1.32 mol of HCl are dissolved in 5.28L of water.
Divide the moles by the Liters.

8. PROBLEM: Dissolve 5.00 g of NiCl2 in enough water to make 250 mL of solution. Calculate the Molarity.
Step 1: Calculate moles of NiCl2
Step 2: Calculate Molarity by Dividing the moles by the volume in Liters.

9. Preparing Solutions
Weigh out a solid solute and dissolve in a given quantity of solvent.
Dilute a concentrated solution to give one that is less concentrated.