1. Solutions Mixtures with a solute and a solvent. How things dissolve…
Solute: the solute is what is being dissolved.
Solvent: the solvent is what is doing the dissolving.
How things dissolve…
“Polar Molecules” are like magnets, one end is positive the other is negative.
Polar molecules can only dissolve other polar molecules.
Non-polar molecules must be dissolved by other non-polar molecules.

2. Polarity

3. Types of Solutions
Solutions may exist as a gas, liquid, or solid depending on the state of matter of the solvent.
Gas solutions
Example – Air Solvent: Nitrogen Solute: Oxygen
Liquid Solutions
Gas in Liquid
Carbonated Water Solvent: Water Solute: Carbon dioxide
Liquid in Liquid
Vinegar Solvent: Water Solute: Acetic Acid
Solid in Liquid
Ocean Water Solvent: Water Solute: NaCl
Solid Solutions
Example – Steel Solvent: Iron Solute: Carbon

4. Solutions as Electrolytes
Solutions of salts, for example NaCl, are good conductors of electricity. Why?
Solutions of acids are also good conductors of electricity. Why?
Solutions of covalent compounds such as sugar are not good conductors of electricity. Why?

5. Solubility
Refers to the maximum amount of solute that will dissolve in a given amount of solvent; at a specified temperature and pressure.
Solubility can usually be expressed in grams of solute per 100 grams of solvent.
NaCl (at 0 degrees Celsius) 35.7g/100 g H2O
(at 20 degrees Celsius) 35.9 g/100 g H2O
(at 40 degrees Celsius ) 36.4 g/100 g H2O

6. Factors that Effect Solubility
Temperature – many substances are more soluble at higher temperatures.
Pressure – solubility increases as a substances external pressure increases.
Surface Area – increasing surface area increases solubility.
Henry’s Law (for gases only): States that at a given temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas.

7. Solubility Curve

8. Solubility Cont.
Saturated Solution – a solution that contains the maximum amount of dissolved solute for a given amount of solvent.
Unsaturated Solution – contains a less dissolved solute for a given temperature and pressure than a saturated solution.
Supersaturated Solution – a solution that has more solute dissolved than it can hold.

9. Solution Concentration
Concentration is a measure of how much solute is dissolved in a specific amount of solvent of solution.
Percent Concentration (%)
Molarity (M) – moles/L
Molality (m) – moles/kg

10. Percent Concentration
Percent by mass formula:
mass (g) of solute
x 100 =
mass (g) of solutions
* percent by volume replace with volume (L) instead of mass
Example: In order to maintain a sodium chloride concentration similair to ocean water, an aquarium must contain 3.6 g of NaCl per 100 g of water. What is the % by mass of NaCl in the solution?

11. Molarity The number of moles of solute per liter (L) of solution.
Molarity (M) Formula:
moles of solute
liters of solution
Example: What is the molarity of a solution produced when 4 moles of NaCl is dissolved by 1000mL of water?

12. Molality
Sometimes we need to use mass because it does not change with temperature.
Molality formula (m):
moles of solute
kilograms of solvent

13. Diluting Solutions
We use this formula in chemistry when we dilute solutions.
Dilution Formula:
M1V1 = M2V2
M = Molarity (M)
V = Volume (L)