1. Solutions (Don’t write what is in parenthesis)
Chapters 12 and 13

2. Universal Solvent – Water
Can dissolve almost every solute
Polar molecule – one end is positive and one is negative.
Shape is bent
(begin with water bubbles)
(Draw – like Mickey Mouse – cup of water)

3. Hydrogen bonding – attraction of water molecules to each other
Hydrogen bonding – attraction of water molecules to each other. Positive end is attracted to negative end.
(Scientists popping water balloons in weightlessness (microgravity) – YouTube)
(Drawing)

4. Capillary action – The ability of water molecules to climb upward on a porous surface.

5. High specific heat capacity – water requires a lot of energy to raise the temperature.
(balloon Demo)

6. Surface tension – Attraction of water molecules at the surface.
(Jar Demo)

7. Solution - Homogeneous mixture = same composition and properties throughout.
Solvent = does the dissolving - most abundant
Solute = substance being dissolved

8. Examples Salt water 14 karat gold Air Solute = Solvent =

9. (Why does water and oil not mix?
“Like dissolves like”
A polar molecule can mix with other polar molecules.
Soluble – capable of being dissolved
Miscible – will mix
Immiscible – will not mix
(Why does water and oil not mix?
Soaps
Vitamins)
(Magic sand)

11. Factors Affecting the Rate of Dissolving
Increased surface area - cube vs. granules
Temperature - different for gases
Agitation

12. (Solubility)
How much solute will dissolve in a certain amount of solvent
(Depends on the nature of the solvent, solute, and temperature)

13. Saturated Solution = contains maximum amount of dissolved solute
Unsaturated = contains less solute than a saturated solution
Supersaturated = solution that contains more dissolved solute than saturated – added solute results in crystallization
Video

14. (When does the solution become saturated?)
(Look at the solubility of the substance = Amount of substance needed to make a saturated solution at a specific temperature)

15. Solubility Curve

16. Electrolyte = conducts electricity due to mobile charges in solution
Nonelectrolytes = do not conduct electricity - no ions formed.

17. Separation processes Dissociation –
- Ionic compound – polar solvent splits existing ions apart.
- Results in a strong electrolyte
Ionization –
- Covalent compound – polar solvent splits molecule apart, creating ions.
- Results in a weak electrolyte

19. Concentration = amount of solute in a given amount of solvent
Molarity (M) = measurement of concentration
M = mol of solute
L of solution

20. Molarity Examples
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution have? (answer 0.4 mol HCl)
What volume of 3.00 M NaCl is needed for a reaction that requires g of NaCl? (answer L)
3.5 L of solution contains 90.0 g of NaCl. What is the solution’ s molarity? (0.441 M)
How many grams of solute are needed to make 2.50 L of a M solution of Ba(NO3)2? (1140 g)

21. Examples:
EXAMPLE: 3.5 L of solution contains 90.0 g of NaCl. What is the solution’ s molarity?

22. You have 0. 8 L of a 0. 5 M HCl solution
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution have?

23. Molality Examples
What is the molality of a solution composed of 255 g of acetone, (CH3)2CO, dissolved in 200. g of water? (22 m)
How many grams of methanol, CH3OH, are required to prepare a solution in g of water? (3.12 g)
What is the molality of a solution containing 18.2 g HCl and 250. g of water? (1.99 m)

24. Taking a concentrated solution and adding water to make it dilute.
Dilutions
Taking a concentrated solution and adding water to make it dilute.
M1 V1 = M2 V2

25. Example
How many mL of a 0.2 M K2Cr2O7 solution is needed to make 100 mL of 0.04 M K2Cr2O7 solution?