1. Solutions

2. Reminder
You have until Friday, May 12 to make up any Gas assignments!!
Check grade to see if you are missing anything
Everything should be updated

3. Seniors You MUST turn in your book before you take the final!!!
Final: Thursday, May 18
Review Packet and Guide

4. Agenda
Solutions Notes
Solubility Curve Practice
SAT Science Reading

5. Talk in your group
What is a solution?
What are some examples?

6. What is a Solution?
A Homogeneous mixture of a solute dissolved in a solvent
Everytime you look, you get the same thing – salt water, Gatorade, etc.

7. Examples of a Solution
Salt or sugar water
Gatorade
Pop (soda)
Everytime you look you get the same thing

8. What is a Solution? Solute: component(s) present in a smaller amount
Solvent: component present in the greatest amount
Assume that it is water, unless stated otherwise
Solvents and solutes can be solids, liquids, or gases
EX: CO2 in pop
EX: acetic acid to make household vinegar compounds
**Does not have to be a solid
Substances that dissolve most readily in water are ionic compounds and polar covalent molecules. As individual solute ions break away from the crystal, the negatively and positively charged ions become surrounded by solvent molecules and the ionic crystal dissolves = solvation. In some ionic compounds, the attractions among the ions in the crystals are stronger than the attractions exerted by water. These compoudns cannot be solvated to any significant extent and are nearly insoluble. Barium sulfate and calcium carbonate

9. Can a solute only be a solid?
Talk about it
Can a solute only be a solid?

10. NOPE! Can be a solid, liquid, or gas!! **CO2 in pop (soda)
**acetic acid to make household vinegar compounds

11. Checkpoint 1: A solution is a:
Heterogeneous mixture of solute dissolved in solvent
Heterogeneous mixture of solvent dissolved in solute
Homogeneous mixture of solute dissolved in solvent
Homogeneous mixture of solvent dissolved in solute C

12. Checkpoint 2:
Which combination is correct? Kool-aid is in the powder, solid form.
Solute
Solvent A
Water
Kool-Aid B
Salt C D
Remember: If not stated, then water is the solvent C

13. Electrolytes
A compound that conducts an electric current when in an aqueous solution or in the molten state
Ions must be mobile, “free,” to carry an electrical current
All ionic compounds

14. What is the Solution Process?
As individual solute ions break away from the crystal, the negatively and positively charged ions become surrounded by solvent molecules and the ionic crystal dissolves = solvation.
In some ionic compounds, the attractions among the ions in the crystals are stronger than the attractions exerted by water causing them to be insoluble. Barium sulfate and calcium carbonate
Barium sulfate and calcium carbonate insoluble

15. What is Solubility?
The maximum amount of solute dissolved in a solvent at a specific temperature

16. There are 3 Types of Solutions:

17. What are types of Solubility?
Unsaturated
Contains less than the maximum amount of solute that a solvent can hold at a specific temperature
Like adding a half of a packet of kool aid to water

18. What are types of Solubility?
Saturated
Contains the maximum amount of solute that a solvent can hold at a specific temperature
Full packet of kool aid

19. What are types of Solubility?
Supersaturated
Contains more than the maximum amount of solute that a solvent can hold at a specific temperature

21. What effects Solubility?
Temperature
Surface Area
Stirring
Pressure (gas)
Amount solvent
Surface area – crush it up, able to dissolve faster
Butter and bread analogy
Stirring – increase the motion and then increase the interaction of molecules
Add more solvent if you have a supersaturated solution
Increase pressure to squeeze molecules closer together in order to have more collisions

22. Checkpoint 3
Which of the following increases the solubility of a solute in a solvent?
Decrease the amount of solvent
Increase the amount of solute
Increase the temperature
Decrease the surface area C
Not B because you want to increase the amount of SOLVENT not SOLUTE

23. Checkpoint 4 Crushing a cube of sugar into small granules:
Increase the surface area and increase solubility
Increases the surface area and decreases solubility
Decreases the surface area and increases solubility
Decreases the surface area and decreases solubility

24. Solubility Curves Used to make a saturated solution in the lab
Tells us what mass of solute will dissolve in 100g of water over a range of temperatures
So how do we know how to make a saturated solution in the lab? We can use solubility curves which tells us what mass of solute will dissolve in 100 g or 100 mL of water over a range of temperatures.

25. Solubility Curves Find the curve for KClO3
At 30°C approximately 10g of KClO3 will dissolve in 100g of water.
If the temperature is increased to 80°C, approximately 40g of the substance will dissolve in 100g (or 100mL) of water.
@30C

26. Checkpoint 5
What mass of KNO3 will dissolve in 100mL of water at 70°C?
0 g
43 g
100 g
140 g

27. Checkpoint 6
What mass of NaCl will dissolve in 100mL of water at 100oC? A. 0 g B. 40 g C. 100 g D. 130 g B

28. Solubility Curves Values on the curve represent saturated solutions
Values on the graph below a curve represent unsaturated solutions
Values above a curve represent supersaturated solutions
All info on the solubility curve is for saturated solutions

29. Checkpoint 7
What term best describes a solution that contains 70g of NaNO3 per 100mL water at 30°C?
Saturated
Supersaturated
Unsaturated

30. Checkpoint 8
What term best describes a solution that contains 60g of dissolved KCl per 100mL water at 80oC? A. Saturated B. Supersaturated C. Unsaturated

31. Concentration The amount of a substance in a given unit of volume
Mass of solute per volume of solution
10 g NaCl in 100 mL water = 10/100 = 0.1g/mL
Percent by mass
10 g NaCl in 100 mL water = 10% NaCl solution
Molarity - Moles of solute dissolved in 1 L of solution
10. g NaCl in 100. mL water =
0.17 moles NaCl / L = 1.7 M

32. Concentration
Concentrated solution – contains a large amount of solute
Dilute solution – contains a small amount of solute

33. Suspensions & Colloids
Heterogeneous mixture
Particles are much larger and do not stay suspended indefinitely
Colloid
Contains particles intermediate in size between those in a solution and those in a suspension
Whipped cream, marshmallow, geletin, milk, mayonnaise, fog, aerosols, dust in air, egg white, jellies, paint, blood
Emulsion – colloid dispersion of a liquid in a liquid