1. Chapters 15 (solutions) and 19 (acids and bases)
Solutions Notes
Chapters 15 (solutions) and 19 (acids and bases)

2. Components of a Solution
Solute:
Solvent:

3. II. Types of Solutions Based on the state of matter of the solvent
Any combination of gas, liquid or solid!
Give examples of 3 different types of solutions:

4. Mothballs – naphthalene (flammable) or 1,4-dichlorobenzene
Brass – copper and zinc
Hydrogen in platinum – hydrogen fuel cells

5. III. Factors Affecting the Rate of Solution
Aqueous
Gas:
Stirring
No stirring or shaking
Heat
Cold temperatures
Small particle size (increases surface area)
Increased pressure
Coca-cola

6. IV. Solubility
Saturated - has all solute that can be dissolved at a given temperature
Unsaturated - can dissolve more solute at that given temperature
Supersaturated - has more solute dissolved than it should at that temperature
Unstable, crystals will form
Rock candy is an example
Supersaturated solution
Supersat 2
Sat vs. unsat

7. IV. Solubility d. What does a solubility curve show?
-show dependence of solubility on temperature
-solids - increase in solubility as temp increases
-gases - decrease in solubility as temp increases
All points “on the line” represent the grams of solute required to form a saturated solution at the given temperature

8. IV. Solubility - Solubility Curve

9. V. How Solutions Form Solvation is the dissolving process
Solvent surrounds solute (based on charges - opposites attract)
Pulls solute into solution
What dissolves in a …
Polar solvent
Nonpolar solvent
General rule:

10. VI. Electrolytes vs. Nonelectrolytes
Electrolyte - forms ions in solution
Conducts electricity
Nonelectrolyte - does not form ions in solution (even if it dissolves)
Does not conduct electricity
A compound is an electrolyte if
Ionic compounds that are soluble in water (must be aqueous, solid ionic compounds are NOT electrolytes)
Acids (formula starts with H)

11. VII. Concentration of Solutions
Concentration Formula - based on definition of concentration and molarity
Molarity = moles of solute per liter of solution
Formula:
If given mass of the substance, you must first convert to moles using molar mass from the periodic table
Must be liters (L) not milliliters (mL)
1L = 1000mL
If given mL, divide by 1000 to get L

12. VII. Concentration of Solutions
b. Examples:
i. What is the concentration if 2.5moles of NaCl is dissolved in 750mL of water?

13. VII. Concentration of Solutions
b. Examples:
ii.What is the concentration if 15.2g of NaCl is dissolved in 500mL of water?

14. VII. Concentration of Solutions
b.Examples
iii.How many liters of a 0.25M solution can be made from 50.0g of CaCl2?

15. VII. Concentration of Solutions
c.Dilution formula - adding water to make a solution more dilute (less concentrated)
-have the same number of moles of the solute, but a larger volume of solvent
Formula:

16. VII. Concentration of Solutions
c. Dilution examples
iv.Calculate molarity if 37.5mL of 12.0M HCl is diluted to mL

17. VII. Concentration of Solutions
c. Dilution examples
v.Calculate molarity if 15.0mL of 6.0M H2SO4 is diluted to mL?

18. VII. Concentration of Solutions
c. Dilution examples
vi.How would you make 500.mL of 1.5M NaCl from a 5.0M stock solution?