1. Solutions Chapter 12 Modern Chemistry
Sections 1-3
Types of Mixtures
The Solution Process
Concentrations of Solution

2. Chapter 12 Section 2 The Solution Process p. 407-417

3. Chapter 12 Section 1 Types of Mixtures p. 401-406
Vocabulary
Solubility
Factors affecting rate of dissolution
Saturated
Unsaturated
Supersaturated
Solubility equilibrium
Solubility values
Dissociation
Hydration
Insoluble
Immiscible
Miscible
Henry’s Law
Effervescence
Chapter 12 Section 1 Types of Mixtures p

4. SOLUBILITY UNSATURATED SATURATED SUPERSATURATED SOLUBILITY EQUILIBRIUM
SOLUBILITY VALUES
SOLUBILITY
FACTORS AFFECTING RATE OF DISSOLUTION
IONIC SOLUTE
LIQUID SOLUTE
GAS SOLUTE
TEMPERATURE
PRESSURE
SOLUBLE
LIKES DISSOLVE LIKES
DISSOCIATION
HYDRATION
MISCIBLE
IMMISCIBLE
INSOLUBLE
HENRY’S LAW
EFFERVESCENCE
Chapter 12 Section 1 Types of Mixtures p
Concept Map 12.2

5. Factors Affecting the Rate of Dissolution
How would you make a solute dissolve faster?
Stir.
Break it up.
Heat it.
Agitate the solution
Increase the surface area of the solute
Heat the solvent
Chapter 12 Section 2 The Solution Process p

6. Factors Affecting Dissolution Rate
Chapter 12 Section 2 The Solution Process p

7. Chapter 12 Section 2 The Solution Process p. 407-417
Solubility
Solubility of a substance is the amount of that substance required to form a saturated solutions with a specific amount of solvent at a specific temperature
Look at the chart on page 410
Dependant on the nature of the solvent and the solute and the temperature of the solute
The maximum amount that can be dissolved is not dependant on the rate it dissolves
in grams
100 g H2O
20° C
Chapter 12 Section 2 The Solution Process p

8. Solubility & Temperature
Chapter 12 Section 2 The Solution Process p
p. 410

9. Solubility and Temperature
Chapter 12 Section 2 The Solution Process p
p. 414*

10. Solubility of Solids in Liquids
Chapter 12 Section 2 The Solution Process p

11. Chapter 12 Section 2 The Solution Process p. 407-417
Solubility
There is a limit to the amount of solute that can be dissolved. Why?
Solubility Equilibrium – the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates.
In other words… the same amount of solute is dissolving and “undissolving” at the same time.
Chapter 12 Section 2 The Solution Process p

12. Solubility & Solution Equilibrium
Chapter 12 Section 2 The Solution Process p

13. Solubility Equilibrium
Insert Holt Disc 2
Chapter 12 Section 2 The Solution Process p

14. Saturated & Unsaturated Solns
Saturated – A solution that contains the maximum amount of dissolved solute.
You can tell that it is saturated because no more solute will dissolve and fall to the bottom of the container.
Unsaturated – A solution that contains less solute than a saturated solution under the existing conditions.
Chapter 12 Section 2 The Solution Process p

15. Mass of Solute Added vs Mass of Solute Dissolved
Chapter 12 Section 2 The Solution Process p
p. 409

16. Supersaturated Solutions
A solution that contains more dissolved solute than a saturated solution contains under the same conditions.
HOW? Saturate a solution. Heat the solution so that more solute can be added. When the solution is cooled undisturbed it will be saturated.
Chapter 12 Section 2 The Solution Process p

17. Unsaturated Saturated Supersaturated
LESS than 35.9g NaCl
in 100g H2O at 20°C
Unsaturated Saturated Supersaturated
EXACTLY 35.9g NaCl
in 100g H2O at 20°C
MORE than 35.9g NaCl
in 100g H2O at 20°C
Chapter 12 Section 2 The Solution Process p

18. Chapter 12 Section 2 The Solution Process p. 407-417
NaC2H3O2 Tower
Insert Holt Disc 2
Chapter 12 Section 2 The Solution Process p

19. Solubility of Compounds
notes
Solubility of Compounds
Chapter 12 Section 2 The Solution Process p

20. Solubility of Compounds
notes
Solubility of Compounds
Chapter 12 Section 2 The Solution Process p

21. Molecule Polarity REVIEW!!
What is the molecule polarity of H2O? CCl4?
How do we determine this?
Insert Holt Disc 2
Chapter 12 Section 2 The Solution Process p

22. Ionic Solute-Solvent Interaction
Ionic solids that dissolve are soluble.
Ionic solids will dissolve in polar solvents but not nonpolar solvents
Water molecules break the crystal lattice into separate ions. This is dissociation.
Then the water molecules surround the ions. This is hydration.
Ionic solids that do not dissolve are insoluble.
Chapter 12 Section 2 The Solution Process p

23. Ionic Solute-Solvent Interaction
Chapter 12 Section 2 The Solution Process p
p. 411

24. Dissociation Animations
Insert Holt Disc 2
Insert Glencoe Disk 2
Chapter 12 Section 2 The Solution Process p

25. Chapter 12 Section 2 The Solution Process p. 407-417
Hydrated Na+
Insert Holt Disc 2
Chapter 12 Section 2 The Solution Process p

26. Liquid Solute-Solvent Interaction
Miscible – Liquids that dissolve freely in one another in any proportion.
Immiscible – Liquids that are not soluble in each other.
“Likes dissolve likes”
Polar solutes dissolve in polar solvents.
Nonpolar solutes dissolve in nonpolar solvents.
Alcohols are slightly polar.
Chapter 12 Section 2 The Solution Process p

27. Miscible and Immiscible
Chapter 12 Section 2 The Solution Process p

28. Chapter 12 Section 2 The Solution Process p. 407-417
Immiscible & Miscible
Chapter 12 Section 2 The Solution Process p
p. 412

29. Chapter 12 Section 2 The Solution Process p. 407-417
How Soap Works
Iodine Solubility
Insert Holt Disc 2
Chapter 12 Section 2 The Solution Process p

30. Gas Solute-Solvent Interactions
Effect of pressure on gas solubility
Pressure changes have little effect on liquid or solid solutes.
Gases dissolved in a liquid are in an equilibrium
This means that some of the gas molecules are going into the solvent and some are going out of the solvent at equal rates.
Chapter 12 Section 2 The Solution Process p

31. Solubility of a Gas in a Liquid
Chapter 12 Section 2 The Solution Process p

32. Gas Solute-Solvent Interactions
Henry’s Law
The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.
Chapter 12 Section 2 The Solution Process p

33. Gas Solute-Solvent Interactions
After being underwater for a long time, a diver will have more gases dissolved in the blood. The diver must pause during the ascent to allow the dissolved gas to come out of solution (the blood) slowly and to be exhaled. If the ascent is too fast the gas can come out of solution while flowing through blood vessels and block essential blood vessels, causing extreme pain, paralysis, or even death.
Chapter 12 Section 2 The Solution Process p

34. Chapter 12 Section 2 The Solution Process p. 407-417
Efervescence
Chapter 12 Section 2 The Solution Process p

35. Keep the fizz in your soda!
Chapter 12 Section 2 The Solution Process p

36. Chapter 12 Section 2 The Solution Process p. 407-417
Mentos and Coke?
Eepy Bird
Steve Spangler Science
Mythbuster
Chapter 12 Section 2 The Solution Process p

37. Gas Solute-Solvent Interactions
Effect of temperature on gas solubility
Increasing temperature decreases the solubility of a gas
An increased temperature increases the kinetic energy so that gas molecules can escape from the solvent
Chapter 12 Section 2 The Solution Process p

38. Chapter 12 Section 2 The Solution Process p. 407-417
Enthalpy of Solution
The net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent.
If heat is given off when the solute dissolves, it is exothermic and the enthalpy is negative.
If heat is taken in when the solute dissolves, it is endothermic and the enthalpy is positive.
Look at the table of enthalpies on page 416.
Chapter 12 Section 2 The Solution Process p

39. Enthalpies of Solutions
Chapter 12 Section 2 The Solution Process p
p. 416

40. Chapter 12 Section 2 The Solution Process p. 407-417
Handheld Heater
Insert Holt Disc 2
Chapter 12 Section 2 The Solution Process p

41. Enthalpies of Solutions
Chapter 12 Section 2 The Solution Process p
p. 415

42. Chapter 12 Section 2 The Solution Process p. 407-417
Ch 12 Sec 2 Homework
Section Review Page 416 # 1-7
Chapter 12 Section 2 The Solution Process p