1. November 14, 2013 Once you’re in, you’re in
November 14, 2013 Once you’re in, you’re in. When the bell rings, electronics and headphones away working on the DO NOW. HAVE OUT ON YOUR DESK YOUR VOCAB HW. TURN IN HW #10. TURN IN ANY LATE STEM PROJECT ASSIGNMENTS AND ANY LATE HW. DO NOW: In the entrance way to the classroom your phase mini-posters are up. On loose-leaf paper record the information from these posters – 4 bullets of info for all 3 phases (Solid, liquid, gas). You have 12 minutes to get this done.

2. Tutoring
Thursday afterschool in 710 (2:30-3:30pm)

3. Homework
Vocabulary column #2 **
HW assignment #11
**graded

4. Week of
11-11: Reaction Stoichiometry Review HW: Anticipation Guide 11-12: Solutions HW: Vocabulary column #1 , assignment # : Solutions HW: Vocabulary colonm #2, assignment # : Reaction Stoich test, Solutions Lab HW: Post-Lab work; study for solutions quiz Monday 11-17

5. Objectives
SWBAT
Infer the quantitative nature of a solution (molarity and dilution)
Summarize properties of solutions
Interpret Solutions diagrams
Explain the solution process

6. Classification of Matter
Solutions are homogeneous mixtures

7. Solute Solvent A solute is the dissolved substance in a solution.
Salt in salt water
Sugar in soda drinks
Carbon dioxide in soda drinks
Solvent
A solvent is the dissolving medium in a solution.
Water in salt water
Water in soda

8. “Like Dissolves Like”
Nonpolar solutes dissolve best in nonpolar solvents
Fats
Benzene
Steroids
Hexane
Waxes
Toluene
Polar and ionic solutes dissolve best in polar solvents
Inorganic Salts
Water
Sugars
Small alcohols
Acetic acid

9. Solubility Trends
The solubility of MOST solids increases with temperature.
The rate at which solids dissolve increases with increasing surface area of the solid.
The solubility of gases decreases with increases in temperature.
The solubility of gases increases with the pressure above the solution.

10. Therefore… Solids tend to dissolve best when: Heated Stirred
Ground into small particles
Gases tend to dissolve best when:
The solution is cold
Pressure is high

11. Solubility Chart

12. Definition of Electrolytes and Nonelectrolytes
An electrolyte is:
A substance whose aqueous solution conducts an electric current.
A nonelectrolyte is:
A substance whose aqueous solution does not conduct an electric current.

13. Electrolytes vs. Nonelectrolytes
The ammeter measures the flow of electrons (current)
through the circuit.
If the ammeter measures a current, and the bulb
glows, then the solution conducts.
If the ammeter fails to measure a current, and the
bulb does not glow, the solution is non-conducting.

14. Try to classify the following substances as electrolytes or nonelectrolytes…
Pure water
Tap water
Sugar solution
Sodium chloride solution
Hydrochloric acid solution
Lactic acid solution
Ethyl alcohol solution
Pure sodium chloride

15. Answers to Electrolytes
NONELECTROLYTES:
Tap water (weak)
NaCl solution
HCl solution
Lactate solution (weak)
Pure water
Sugar solution
Ethanol solution
Pure NaCl

16. Foldable: Solution = Solute + Solvent
Solute - gets dissolved
Solvent - does the dissolving
Aqueous (water)
Tincture (alcohol)
Amalgam (mercury)
Organic
Polar
Non-polar
Solutions are always homogeneous – evenly mixed.
Solutions
– In all solutions, whether gaseous, liquid, or solid, the substance present in the greatest amount is the solvent, and the substance or substances present in lesser amounts are the solute(s).
– Solute does not have to be in the same physical state as the solvent but the physical state of the solvent determines the state of the solution.
– If solute and solvent combine to give a homogeneous solution, solute is said to be soluble in the solvent.
The difference between hydrophilic and hydrophobic substances has substantial consequences in biological systems.
– Vitamins can be classified as either fat soluble or water soluble.
1. Fat-soluble vitamins (Vitamin A) are nonpolar, hydrophobic molecules and tend to be absorbed into fatty tissues and stored there.
2. Water-soluble vitamins (Vitamin C) are polar, hydrophilic molecules that circulate in the blood and intracellular fluids and are excreted from the body and must be replenished in the daily diet.
Nightmare on White Street
Chem Matters, December 1996

17. Calculations of Solution Concentration: Molarity
Molarity is the ratio of moles of solute to liters of solution
Practice problems on handout

18. Diluting Solutions
When you add solvent, you increase the number of solvent particles among which the solute particles move
Moles of solute in stock solution = moles of solute after dilution
M1V1 = M2V2
Practice problems on handout

19. Mr. Causey Video Guide

20. Colligative Properties of Solutions
Colligative properties are properties that depend only on the number of solute particles in solution and not on the nature of the solute particles.
Vapor Pressure Lowering
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure

21. FOLDABLE 4 squares Colligative Properties
Vapor Pressure Lowering
Vapor Pressure Lowering is due to the number of solute particles in solution
The greater the number of solute particles in a solvent, the lower the resulting vapor pressure.
Boiling Point Elevation
Temperature difference between as solution’s boiling point and a pure solvent’s boiling point
The greater the number of solute particles in the solution, the greater the boiling point elevation.

22. Colligative Properties
Freezing Point Depression
The difference in temperature between its freezing point and the freezing point of its pure solvent.
The freezing point of a solution is always lower than that of a pure solvent.
Depends on the number of solute particles in a given volume of solution.
Osmotic Pressure
Amount of additional pressure caused by the water molecules that moved into the solution.
Depends on the number of solute particles in a given volume of solution.

23. Complete the following using your notes and your book by Monday 11-18
Solubility Curve Worksheet
Stoich using molarity worksheet (you will receive tomorrow)
Net ionic equation handout

24. Exit Ticket
1. What volume, in milliliters of 2.00M calcium chloride (CaCL2) stock solution would you use to make .50L of .300M calcium chloride solution?
2. A mL intravenous solution contains 5.10g of glucose (C6H12O6). What is the molarity of the solution? Molar mass of glucose is 180g.