1. Mixtures (Solutions) Heterogeneous Homogeneous Solution Heterogeneous
colloid
Heterogeneous
suspension

2. Colloid
Solution

3. + = = + Solutions Salt water Carbonated water Solution Solute Solvent
Most common solvent = water
Solution with water as solvent is aqueous solvent

4. Solvation Water molecules in continuous motion
Water molecules in continuous motion
Water molecules collide with crystals if solid
Solvent water molecules attract the solute ions (Na+, Cl-)
As individual ions break away from the crystal, the sodium chloride dissolves

5. Dissolving Like dissolves like
nonpolar
Like dissolves like
Solute and solvent need to have similar polarities to be soluble
Polar
Polar dissolves polar
Nonpolar dissolves nonpolar
Polar dissolves ionic

7. Rate of Dissolving Most often increases with: Stirring (agitation)
Temperature
Surface area
Contact of solute with solvent
Faster b/c more surface area

9. Solubility The amount of substance that
dissolves in a given quantity of
solvent at a given temperature.
Saturated
Contains maximum amount of solute for given amount of solvent at given temperature
Some solute particles out of solution
Unsaturated
Solution contains less solute than saturated solution
All solute particles in solution

10. Supersaturated

11. Solubility of Gas Gases more soluble at lower temperatures
Gases more soluble at higher pressures
Soda has large amounts of CO2 dissolved in water

12. Molarity
Molarity (M) = (moles of solute)/(Liter of solution)
Measures concentration
Practice:
If 44 grams of sodium fluoride are dissolved to make a 3.5M solution, what is the volume of the solution?

13. Dilutions To dilute a solution, more SOLVENT is added
Moles of SOLUTE is the same
Moles before = moles after
M1V1 = M2V2
Practice:
How many liters of 15 molar HCl are need to make 400 mL of a 0.4 molar solution of HCl?