1. Solutions

2. Types of Mixtures Three types of mixture Solutions Colloids
Homogeneous
Colloids
Heterogeneous
Suspensions

3. Solutions Solutions are made of two parts Solute The process Solvent
Substance that is being dissolved
Solvent
Substance the is doing the dissolving
The process
Solvent particles surround the solute particles
Energy associated the process

4. Factors that affect solutions
Temperature
Increasing the kinetic energy of the solvent particles will allow the solvent to surround more solute particles
Faster moving particles creates more contact
Stirring or agitation
Creating contact between the solvent and solute will allow dissolution to occur at a faster rate

5. Factors that affect solutions
Surface area
Creating more surface area of the solute allows for contact with the solvent
Amount of particles
More particles of the solvent can dissolve more solute

6. Types of solutions Six types Solid dissolving solid
Liquid dissolving liquid
Gas dissolving gas
Liquid dissolving gas
Liquid dissolving solid
Solid dissolving liquid

7. Dental amalgam
Mixture of mercury and silver

8. Colloids
Heterogeneous mixture where the mixed particles are too large to be dissolved but small enough to not settle to the bottom
Produces the Tyndall Effect
Scatters light when shone through the mixture

9. Tyndall effect
Particles are large enough to cause light to scatter as it passes through the mixtures

10. Suspensions Large particles are temporary suspended in the mixture
Settles out over time

11. Videos
examples.html

12. Electrolyte and Nonelectrolyte
Electrolytes are solutions that contain free radicals
Solute such as acids, bases, and ionic compounds
Nonelectrolytes do not contain free radicals
Molecular compounds typically work in this manner

13. Solubility Qualitative measurements Saturated Unsaturated
Contains the maximum amount
Unsaturated
Contains less than the maximum amount
Supersaturated
Contains more than the maximum amount

14. Solubility
Solubility is the amount of solute that can be dissolved in a give amount of solvent
Establishes a ratio between the two parts
Table 4 page 410

16. Solubility examples

17. Concentrations of solutions
Molarity
Expressed as moles of solute per liters of solution
Molality
Expressed as moles of solute per kilograms of solvent

18. Examples of concentrations

19. Solute solvent interactions
Liquids-liquid interactions
Liquids that dissolve each other are known as miscible
Liquids that do not dissolve each other are immiscible
Ionic compounds
Ionic solutes go through a process of dissociation when that go into solution
This process increases the total number of particles in solution

20. Solute solvent interactions
Gas solutes
When gases are dissolved in liquids, the factors that affect the solution are changed
The partial pressure at the surface of the liquid forces particles of the gas to go into solutions
Known as Henry's Law
Ratio between solubility and pressure
Temperature must also be lowered to help keep the gas in solution

21. Solute solvent interactions
Temperature for solid and liquid solutes
Typically solids and liquids will be more soluble when temperature is increased but the degree of the increase is not uniform
Also not all will increase with temperature