1. Ch. 24 - Solutions I. How Solutions Form Definitions
Types of Solutions
Dissolving
Rate of Dissolving

2. A. Definitions Solution - homogeneous mixture
Solute - substance being dissolved
Solvent - present in greater amount

3. A. Definitions
Solute - KMnO4
Solvent - H2O

4. B. Types of Solutions Based on state of solvent.
All solid-liquid-gas combos are possible.
EX: dental amalgam (alloy of silver, mercury, etc.)
liquid solute, solid solvent
solid solution

5. C. Dissolving Solvation occurs at the surface of the solute
solvent particles surround solute particles (+/- attraction)
solute particles are pulled into solution

6. NaCl dissolving in water
C. Dissolving
NaCl dissolving in water

7. D. Rate of Solution Solids dissolve faster... more stirring
small particle size (increased surface area)
high temperature

8. D. Rate of Solution Gases dissolve faster... no shaking or stirring
high pressure
low temperature

9. II. Solubility & Concentration
Ch Solutions
II. Solubility & Concentration

10. A. Concentration Concentrated solution large amount of solute
Dilute solution
small amount of solute

11. A. Concentration % by Volume usu. liquid in liquid
EX: 10% juice = 10mL juice + 90mL water
% by Mass
usu. solid in liquid
EX: 20% NaCl = 20g NaCl + 80g water

12. A. Concentration UNSATURATED SOLUTION more solute dissolves
no more solute dissolves
SUPERSATURATED SOLUTION
becomes unstable, crystals form
concentration

13. B. Solubility Solubility
maximum grams of solute that will dissolve in 100 g of solvent at a given temperature
varies with temperature
based on a saturated solution

14. B. Solubility Solubility Curve
shows the dependence of solubility on temperature

15. B. Solubility Solids are more soluble at... high temperatures.
Gases are more soluble at...
low temperatures.
high pressures (Henry’s Law).

16. III. Particles in Solution
Ch Solutions
III. Particles in Solution
“Like Dissolves Like”
Electrolytes
Colligative Properties

17. A. “Like Dissolves Like”
NONPOLAR
POLAR
Detergents
polar “head” with long nonpolar “tail”
can dissolve both types

18. B. Electrolytes Electrolyte Weak Electrolyte Non- Electrolyte+
salt - +
acetic acid - +
sugar
Electrolyte
Weak
Electrolyte
Non-
Electrolyte
solute exists as
ions only
solute exists as
ions and
molecules
solute exists as
molecules only

19. B. Electrolytes Dissociation
separation of +/- ions when an ionic compound dissolves in water

20. B. Electrolytes Ionization
breaking apart of polar covalent molecules into ions when dissolving in water

21. C. Colligative Properties
properties of solutions that depend only on solute concentration
Freezing Point Depression
solutes lower the f.p. of a solvent
Boiling Point Elevation
solutes raise the b.p. of a solvent

22. C. Colligative Properties
Freezing Point Depression
View Flash animation.

23. C. Colligative Properties
Boiling Point Elevation
Solute particles “get in the way.”

24. C. Colligative Properties
Effect increases as the solute concentration increases.
Uses:
antifreeze
making ice cream
salting icy roads

25. IV. Intro to Acids & Bases Definitions Properties Uses
Ch Acids & Bases
IV. Intro to Acids & Bases
Definitions
Properties
Uses

26. HCl + H2O  H3O+ + Cl– A. Definitions Acids
Ionize to form hydronium ions (H3O+) in water
HCl + H2O  H3O+ + Cl–

27. NH3 + H2O  NH4+ + OH- A. Definitions Bases
Dissociate or ionize to form hydroxide ions (OH-) in water
NH3 + H2O  NH4+ + OH-

28. A. Definitions Indicator
substance that changes color in an acid or base
Examples:
litmus - red/blue
phenolphthalein - colorless/pink
goldenrod - yellow/red
red cabbage juice - pink/green

29. B. Properties ACIDS BASES sour taste corrosive electrolytes
turn litmus red
react with metals to form H2 gas
bitter taste
corrosive
electrolytes
turn litmus blue
slippery feel

30. C. Uses ACIDS H3PO4 - soft drinks, fertilizer, detergents
H2SO4 - fertilizer, car batteries
HCl - gastric juice
HC2H3O2 - vinegar

31. C. Uses BASES NaOH - lye, drain and oven cleaner
Mg(OH)2 - laxative, antacid
NH3 - cleaners, fertilizer

32. . Strength of Acids & Bases Strong vs. Weak pH
Ch Acids & Bases
. Strength of Acids & Bases
Strong vs. Weak pH

33. V. Intro to Acids & Bases Definitions Properties Uses
Ch Acids & Bases
V. Intro to Acids & Bases
Definitions
Properties
Uses

34. HCl + H2O  H3O+ + Cl– A. Definitions Acids
Ionize to form hydronium ions (H3O+) in water
HCl + H2O  H3O+ + Cl–

35. NH3 + H2O  NH4+ + OH- A. Definitions Bases
Dissociate or ionize to form hydroxide ions (OH-) in water
NH3 + H2O  NH4+ + OH-

36. A. Definitions Indicator
substance that changes color in an acid or base
Examples:
litmus - red/blue
phenolphthalein - colorless/pink
goldenrod - yellow/red
red cabbage juice - pink/green

37. B. Properties ACIDS BASES sour taste corrosive electrolytes
turn litmus red
react with metals to form H2 gas
bitter taste
corrosive
electrolytes
turn litmus blue
slippery feel

38. C. Uses ACIDS H3PO4 - soft drinks, fertilizer, detergents
H2SO4 - fertilizer, car batteries
HCl - gastric juice
HC2H3O2 - vinegar

39. C. Uses BASES NaOH - lye, drain and oven cleaner
Mg(OH)2 - laxative, antacid
NH3 - cleaners, fertilizer

40. A. Strong vs. Weak Strong Acid/Base 100% ions in water
strong electrolyte
HCl, HNO3, NaOH, LiOH - +
Weak Acid/Base
few ions in water
weak electrolyte
HC2H3O2, NH3 - +

41. B. pH Scale pH a measure of the concentration of H3O+ ions in solution
measured with a pH meter or an indicator with a wide color range 7
INCREASING
ACIDITY
NEUTRAL
BASICITY 14

42. pH of Common Substances
B. pH Scale
pH of Common Substances

43. ConcepTest
Which of the following "molecular" pictures best represents a concentrated solution of the weak acid HA? A B

44. ConcepTest Is the following statement TRUE or FALSE?
A strong acid has a lower pH than a weak acid.
FALSE - Strong/weak refers to amount of ionization whereas pH refers to concentration of H+.

45. Ch. 24 - Acids & Bases VI. Neutralization Neutralization Reaction
Titration

46. A. Neutralization Reaction
Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.

47. A. Neutralization Reaction
ACID + BASE  SALT + WATER
HCl + NaOH  NaCl + H2O =
Neutralization does not always mean pH = 7.

48. A. Neutralization Reaction
KOH + HNO3  H2O + KNO3
Acid?
Base?
Salt?
HNO3
KOH
KNO3

49. B. Titration
standard solution
unknown solution
Titration
Process in which a standard solution is used to determine the concentration of an unknown solution.

50. B. Titration Endpoint (equivalence point)
Point at which equal amounts of H3O+ and OH- have been added.
Determined by…
indicator color change
dramatic change in pH

51. VI. Naming Acids Definition Acid Names Acid Formulas
Ch Chemical Bonds
VI. Naming Acids
Definition
Acid Names
Acid Formulas

52. A. Definition Acid Compound that forms H+ in water.
Formula usually begins with ‘H’.
Examples:
HCl, HNO3, H2SO4

53. B. Acid Names

54. B. Acid Names HBr H2CO3 -ide  hydrobromic acid H2SO3 -ate
 carbonic acid
-ite
 sulfurous acid

55. C. Acid Formulas hydrofluoric acid sulfuric acid nitrous acid -ide
 HF
-ate
 H2SO4
-ite
 HNO2