1. Bellwork 1. What do you remember about the difference between homogeneous mixtures and heterogeneous mixtures?

2. Heterogeneous mixtures are not the same throughout.
A suspension is a mixture that looks uniform when stirred or shaken, but separates into different layers when it is no longer agitated.
A colloid is a mixture of very tiny particles that are dispersed in another substance but do not settle out of the substance.

3. Homogeneous mixtures look the same through out.
Vinegar and oil salad dressing is an example of what type of mixture?
Some immiscible liquids can mix together in emulsions.
Mayonnaise is an example of two immiscible liquids, vinegar and oil, that can be mixed together with an emulsifier, and egg yolk.
Homogeneous mixtures look the same through out.
All solutions are example of homogeneous mixtures. They are a group of molecules that are mixed up in a complete even distribution.
The solute is the substance that is being dissolved in the solution
The solvent is the substance that does the dissolving

4. Chocolate
milk
Carbonated
water
Alloys

6. Solubility
6. Solubility is the ability of the solvent to dissolve the solute.
a. What factors affect solubility?
Miscible: when 2 liquids dissolve(ex: alcohol and water)
Temperature
Pressure
Structure of
the substance

7. Solubility
6. Solubility is the ability of the solvent to dissolve the solute.
a. What factors affect solubility?
Stirring (agitation)
Surface area

8. 7. “Like dissolves like”
Polar substances dissolve other polar substances, but cannot dissolve nonpolar substances.
For example oil and water don’t mix because water is polar and oil is nonpolar.
8. Solutions can have different concentrations depending on how much solute and solvent is present.
A dilute solution has very little solute dissolved in a large amount of solvent.
A concentrated solution has a lot of solute dissolved in a solvent.

9. 9. We can also classify solutions based on amount of solute.
a. Unsaturated solutions 
have less than the maximum amount of solute dissolved in them. (This means that more solute could be added and the solute would still dissolve!)
b. Saturated solutions 
have the maximum amount of solute dissolved in them. No more can be made to dissolve.
c. Supersaturated solutions 
have more than the maximum amount of solute dissolved in them. This is not possible for all solutions!
How do you think we could create a supersaturated solution?

10. See the images of the seating on a bus
See the images of the seating on a bus. Using the vocabulary describing solutions, which is unsaturated, supersaturated, and which is saturated?
Saturated
Unsaturated
Supersaturated

11. Solubility Curve NH3 KNO3 KI 50g per 100 60°C supersaturated
Which salt is least soluble in water at 60oC? ___________________
Which salt shows the greatest increase in solubility from 0-60oC? _______
At 50oC, 70 g of KNO3 is dissolved in 100 g of water. Is the solution saturated, unsaturated or supersaturated? ___________________
Which is the most soluble salt at 20oC? ___________________
What is the solubility of KCl at 80oC? ___________________
What it the temperature at which KNO3 has a solubility of 90g/100g of water? ________________
NH3
KNO3
supersaturated KI
50g per 100
60°C

12. Solubility Curve NaNO3 NaCl KClO3 35g / 100 20°C Unsaturated – barely!
Which salt is most soluble in water at 60oC? ___________________
Which salt shows the least increase in solubility from 0-60oC? _______
At 50oC, 40 g of KCl is dissolved in 100 g of water. Is the solution saturated, unsaturated or supersaturated? ___________________
Which is the least soluble salt at 20oC? ___________________
What is the solubility of KCl at 20oC? ___________________
What it the temperature at which KNO3 has a solubility of 20g/100g of water? ________________
NaNO3
NaCl
Unsaturated – barely!
KClO3
35g / 100
20°C

13. The Chemistry of Acids and Bases
To play the movies and simulations included, view the presentation in Slide Show Mode.

14. Acid and Bases

15. Acid and Bases

16. What is an acid?
An acid is a solution that has an excess of H+ ions. It comes from the Latin word acidus that means "sharp" or "sour".
The more H + ions, the more acidic the solution.

17. Properties of an Acid Tastes Sour Conduct Electricity
Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin and paper
Some acids react strongly with metals – Tomatoes turn Aluminum foil black.
Turns blue litmus paper red
Picture from BBC Revision Bites

18. Properties of an Acid
Neutralize with a base if they are the same concentration
Strong acids fully ionize in water.
Weak acids have fewer hydrogen ions in solution.
Picture from BBC Revision Bites

19. Uses of Acids Acetic Acid = Vinegar
Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch.
Ascorbic acid = Vitamin C which your body needs to function.
Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics.
Car batteries

20. What is a base? A base is a solution that has an excess of OH- ions.
Another word for base is alkali.

21. Properties of a Base Feel Slippery Taste Bitter Corrosive
Can conduct electricity. (Think alkaline batteries.)
Do not react with metals.
Turns red litmus paper blue.

22. Uses of Bases
Bases give soaps, ammonia, and many other cleaning products some of their useful properties.
The OH- ions interact strongly with certain substances, such as dirt and grease.
Chalk and oven cleaner are examples of familiar products that contain bases.
Your blood is a basic solution.

23. pH Scale pH means “potential hydrogen”
pH is a measure of how acidic or basic a solution is.
The pH scale ranges from 0 to 14.
Acidic solutions have pH values below 7
A solution with a pH of 0 is very acidic.
A solution with a pH of 7 is neutral.
Pure water has a pH of 7.
Basic solutions have pH values above 7.