1. Matter (Review and New)
Recall that all matter can be classified as a mixture or a substance. Up to now we have concentrated on how to classify matter as substances (elements and compounds).
Now, we are going to concentrated on how to classify mixtures.

2. Heterogeneous Mixtures
There are two types of heterogeneous mixtures: suspensions and colloids

3. Suspensions Particles are evenly dispersed
Particles in suspensions may be filtered out
ex: you can separate sand and water
Particles may settle out (separate) and are large in size
1) Immiscible liquids do not mix
ex: oil and water
a) immiscible liquids can be separated by pouring the less dense liquid off the top (called decanting)

4. Particle Size Suspensions > Colloids > Solutions
Particles are smaller than the particles in suspensions but are larger than the particles in a solution
Particles cannot be filtered
Particles do not settle out
Tyndall effect  scattering of light by a colloid
Particle Size Suspensions > Colloids > Solutions

5. Examples of colloids: gelatin desserts, whipped cream, smoke, and fog
Emulsion is a colloid in which liquids that normally do not mix are spread throughout each other
Examples:
1) Mayonaise  egg yolk holds oil and vinegar together
2) Bile  allows your body to breakdown fat
a) emulsifier  substance that holds the immiscible liquid together

6. Homogeneous Solutions (Solutions)
Homogeneous mixtures are uniform throughout; all samples are the same
All homogeneous mixtures are solutions
A solution is a homogeneous mixture of two or more substances uniformly dispersed throughout a single phase
Solutions are made of solutes and solvents
1) solute – what is dissolved
2) solvent – what does the dissolving; present in the greatest amount

7. Miscible Liquids mix to form solutions
Miscible is defined as 2 or more liquids that form a single layer when mixed
Ex: rubbing alcohol (water and isopropanol)
Miscible liquids can be separated by distillation (boiling off one liquid)
a) Distillation only works with liquids that have different boiling points

8. Other States of Matter (beside liquids) can form solutions
Many common solutions are solids dissolved in liquids (salt water)
Solutions can be made by dissolving a liquid in another liquid (vinegar is made of acetic acid dissolved in water)
Gases dissolved in gases are solutions (air)
Gases can be dissolved in liquids (CO2 dissolved in water gives soda the fizz)

9. 5) Gases can be dissolved in solids to make solutions (moth balls)
6) Solids dissolved in solids make a solution (brass is made of copper and zinc)
a) An alloy defined as a solid or a liquid mixture of two or more metals.

10. Solutions
A solution is a mixture that has the same composition, color, density, and taste throughout.
The atoms in a solution are evenly spread out.
Solutions are homogeneous

11. Phases of Solutions
Solutions can exist in the solid, liquid, and gas phases
All mixtures of gases are solutions, including air
Solutions in the solid phase are called alloys.
Examples of alloys are:
Brass, coins

13. Solutes and Solvents Solute is the substance that is being dissolved.
Solvent is what does the dissolving (typically water)
Example: Salt water
Salt is the solute
Water is the solvent

14. Water: A polar molecule
Polar  slightly positive and slightly negative ends
Because water is a polar molecule, it is known as the Universal Solvent
Oxygen end has a slightly (-) charge, Hydrogen has a slightly (+) charge. O- H+ H+

15. Dissolving a Solid in a Liquid
Dissolving salt in water.
NaCl is held together by an ionic bond. However, the Cl end is more negative than the Na end.
Step One
The moving water molecules collide with the salt molecules as the water’s negative ends are attracted to the positive ends of the salt molecules.
Cl-
Na+ H+
Cl- H+
Na+ O- O- H+ H+

16. Step Two:
The water molecules surround and pull the salt molecule apart creating Na+ and Cl- into solution.
The attractive forces between the water and salt molecules are stronger than the forces holding the NaCl molecule together. H+ H+ O-
Cl-
Na+ O- H+ H+

17. Step Three
The water molecules and salt molecules spread out to form a homogeneous solution.
The process continues until all the salt molecules have dissolved.

18. Non polar Molecules
Non polar materials have no positive or negative ends.
Are not attracted to water, so they do not dissolve easily in water
Examples: oil, soap

19. Rate of Dissolving
Stirring will increase the dissolving rate. By stirring a solution, more fresh solvent comes into contact with the solute.
Crushing the solvent will increase the dissolving rate. Crushing creates more surface area for the solvent to interact with.
Increasing the temperature will also increase the dissolving rate. Increasing the temperature speeds up the movement of the solute molecules creating more solute/solvent collisions

20. How much can dissolve?
Solubility is the maximum amount of solute that can be dissolved in a given amount of solvent at a given temperature.
Each beaker contains the same amount of water and water of the same temperature. Only 1g of “A” dissolves in 100 mL of water, but more than 3g of “B” dissolves in the same amount of water at the same temperature. Substance B is more soluble.

21. Solubility Curves
Compare the solubility of different substances at different conditions
Notice that for most solutes, as temperature increases more solute is able to dissolve.

22. How much potassium nitrate will dissolve at 80°C in 100 g of water?

23. How much potassium nitrate will dissolve at 80°C in 100 g of water?

24. At what temperature will 100 g of potassium bromide dissolve in 100 g of water?

25. At what temperature will 100 g of potassium bromide dissolve in 100 g of water?
95°C

26. Concentration
Concentrated solution  large amount of solute in the solvent
Dilute solution  small amount of solute in the solvent
“watered down”

27. Types of Solutions
Saturated Solutions  contains all the solute it can hold at a given temperature.
Unsaturated Solutions  can dissolve more solute at a given temperature.
Supersaturated Solution  contains more solute than a saturated solution at the same temperature
a) unstable  if you disturb them, crystals will form

28. The Solubility of Gases
Depend on the temperature and pressure
Increase temperature then solubility of gas decreases because the gas molecules move around faster and escape the liquid.
Increase pressure then solubility of gas increases because the pressure holds the gas molecules in the liquid.

29. Gas solubility and fish
Amount of oxygen gas in water decreases as temperature increases.
Fish will go to the bottom of ponds or lakes during warm weather because that is where the oxygen is located.