1. Mixtures Heterogeneous mixtures Homogeneous mixtures
Components in different phases
Homogeneous mixtures
All components in same phase

2. Solutions Homogeneous mixture
Most commonly a solid dissolved in a liquid
Gaseous solutions
air
Solid solutions
Alloys

3. Dissolving process
Solute – the component that gets dissolved; the compound in the smaller amount
Solvent – the component that does the dissolving; the compound in the larger amount

4. Dissociation – the process in which a solid dissolves in a liquid
Depends on polarity
Solvent usually water
Polar water molecules are attracted to other polar molecules and to ions
Non-polar molecules are attracted to other nonpolar molecules

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Hydration – water molecules surround the other molecules until the attraction between the water and the ion is stronger than the crystal

6. Dissociation
Individual molecules or ions are pulled away from each other
Solvation – the surrounding of the solute particles
Once dissociation occurs the ions of the compound act independently

7. Miscibility Whether or not two liquids will form a solution
Miscible liquids are mutually soluble
Like dissolves like

8. Factors that affect solubility
Temperature
Solids generally more soluble in liquids at higher temperature
Gases more soluble in liquids at lower temperatures

9. Nature of the solvent/solute
Pressure
Henry’s law – at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid
Nature of the solvent/solute
Polarity
Molecular size/structure

10. Factors that affect rate of solution
Temperature
Agitation
Particle Size
Surface area
Concentration
Saturated
Unsaturated
Supersaturated

11. Solubility Curves
Used to predict the conditions under which substances will form solutions

12. At 0.0°C, which is more soluble, NaCl or KBr?
True or false, temperature has a significant effect on the solubility of NaCl.
Which of these dissolutions would have the highest value for heat of solution
What would be the approximate value of the heat of solution for NaCl?

13. At what temperature will 140g of NaClO3 dissolve in 100g of water?

14. Physical Properties Review
Properties that can be measured without changing the substance
Intrinsic properties
Properties that do not change when the amount of substance changes
Density, boiling point, freezing point
Extrinsic properties
Properties that change with a change in the amount of substance
Volume shape size

15. Dissociation of solute particles
Ionic solute particles dissociate in solution and act independently
Covalent bonds are not usually broken in solution
So covalently bonded molecules will almost always be treated as one particle

16. Concentration Saturated Unsaturated Supersaturated
Contains the normal amount of solute
Unsaturated
Contains less than the normal amount of the solute
Supersaturated
Contains more solute than normal