1. Solutions

2. BASIC DEFINITIONS
Solution – a homogeneous mixture of 2 or more substances in a single phase
Phase- solid, liquid, gas
Mixture – blend of 2 or more pure substances not chemically combined
heterogeneous mixture-visibly different parts

3. A heterogeneous mixture is a mixture where the components of the mixture are not uniform.
In other words, you can see the different components that make up the mixture.
A homogeneous mixture is a mixture where the components that make up the mixture are uniformly distributed throughout the mixture. The composition of the mixture is the same throughout. 
In other words, you can’t see the different components that make up the mixture.

4. Solute - substance being dissolved
Solute – The dissolved substance usually in smaller amount
Solvent – the dissolving medium usually in larger amount
Solute - substance being dissolved
Solvent - present in greater amount

5. Solubility Definition:
the maximum quantity of a substance that may be dissolved in another.
-The maximum amount of solute that may be dissolved in a solvent .

6. FACTORS AFFECTING SOLUBILITY
Surface Area – increasing the surface area gives molecules more places to interact causing the solute to dissolve faster
Agitation/Stirring – stirring gives molecules more opportunities to interact – faster dissolving
Temperature – Adding heat adds energy to molecules = faster dissolving
“Like dissolves like” – polar solutes dissolve in polar solvents or Nonpolar solutes dissolve in Nonpolar solvents

7. Solutes Change Solvents
The amount of solute in a solution determines how much the physical properties of the solvent are changed.
Lowering the Freezing Point
Raising the Boiling Point
The freezing point of a liquid solvent
decreases when a solute is dissolved in it.
Ex. Pure water freezes at 320F (00C), but when salt is
dissolved in it, the freezing point is lowered.
This is why people use salt to melt ice.
The boiling point of a solution is higher
than the boiling point of the solvent.
Therefore, a solution can remain a liquid at
a higher temperature than its pure solvent.
Ex. The boiling point of pure water is 2120F (1000C),
but when salt is dissolved in it, the boiling
point is higher. This is why it takes salt water
longer to boil than fresh water.

8. CONCENTRATION MOLARITY (M) The strength of a solution
Moles of solute per Liter of solution

9. SAMPLE PROBLEM A
You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity of that solution?

10. SAMPLE PROBLEM A
You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity of that solution?
Step 1: Outline what you know.
M = ? Mol / L
mol = 90.0 g
L = 3.50 L

11. SAMPLE PROBLEM A
You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity of that solution?
Step 2: Convert any units necessary.
mol = 90.0 g NaCl
1 mol NaCl
90.0 g NaCl x
1.54 mol NaCl =
58.44 g NaCl

12. SAMPLE PROBLEM A
You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity of that solution?
Step 3: Plug into the equation and solve.
M = ? Mol / L
mol = 1.54 mol
L = 3.50 L

13. SAMPLE PROBLEM A
You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity of that solution?
Step 3: Plug into the equation and solve.
1.54 mol =
M =
0.44 mol / L
3.50 L

14. SAMPLE PROBLEM B
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?

15. SAMPLE PROBLEM B
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
Step 1: Outline what you know.
M = 0.5 Mol / L
mol = ? mol
L = 0.8 L

16. SAMPLE PROBLEM B
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
Step 2: Convert any units necessary.
All units correct! Moving on…

17. SAMPLE PROBLEM B
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
Step 3: Plug into the equation and solve.
M = 0.5 Mol / L
mol = ? mol
L = 0.8 L

18. SAMPLE PROBLEM B
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
Step 3: Plug into the equation and solve.
HINT- Cross multiply!!! X
(0.8 L)
0.5 M =
(0.8 L) 1
0.8 L

19. SAMPLE PROBLEM B
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
Step 3: Plug into the equation and solve.
mol = 0.4