1. Chapter 7: Solutions

3. Section 1: Solutions and Other Mixtures
Heterogeneous: a mixture with no fixed composition, not the same throughout
Examples:
Suspension: particles are more or less evenly dispersed, particles can settle and even be filtered. Ex: orange juice
Colloid: like a suspension but the particles are smaller (and scatter light). Ex: paint
Emulsions: droplets of fats or lipids dispersed in water. Ex: cream

4. Mixtures: (cont) Homogeneous Mixtures: uniform, the same throughout
Components: solute and solvent like salt and water
Solutions can be liquid, solid or gas
Alloys are solutions of metals
Quiz
Quiz 2

5. Examples of Solutions gas in gas air ( N2, O2 , Ar, CO2 , other gases)
gas in liquid soda pop (CO2 in water)
liquid in liquid gasoline (a mixture of hydrocarbon compounds)
solid in liquid sea water ( NaCl and other salts in water)
gas in solid H2 in platinum or palladium
liquid in solid dental amalgams ( mercury in silver)
solid in solid alloys: brass, (Cu/Zn), solder (Sn/Pb)

6. Section 2: How substances dissolve
Water:
A common solvent
Polar compounds like water,
dissolve ions and polar molecules
Hydrogen bonding occurs between water molecules and helps to dissolve some polar molecular compounds
Like dissolves like, nonpolar compounds dissolve nonpolar compounds

7. Dissolving Process Solutes with a larger surface area dissolve faster
Stirring and shaking help to increase solution rate
An increase in temperature increases the solubility of some solids
Solutes can affect the physical properties of a solution

8. Section 3: Solubility and Concentration
Terms:
Soluble
Insoluble
Unsaturated
Saturated
Supersaturated
Solubility of substances (in grams) is often measured in 100 g (or 100 mL) of water

9. Factors affecting solubility
Substance dependent: some substances dissolve in water and some do not
Temperature affects solubility
Solids
Gases
Pressure affects solubility of gases

10. Solubility Curves

11. Solubility of Gases

12. Measuring solubility Concentration: g/100 mL of solvent
Molarity: moles of solute/L of solution
mol/L = M
p 243
Examples: