1. Acids
Lesson 1
Acid and Base
Theories Properties
Page 109

2. Acid Base Theories

3. Acid Base Recap
Discuss with your partner and come up with 5 things that you remember about acids and bases

5. Acids produce H+ in solution,
example: HCl
Bases produce OH- in solution,
example NaOH

6. ACIDS Acids often behave like acids only when dissolved in water.
Therefore, acids often are written with symbol (aq) = aqueous = water.
The chemical formula of an acid usually starts with hydrogen (H).
HCl(aq) = hydrochloric acid, HNO3(aq) = nitric acid
Acids with a carbon usually have the C written first.
CH3COOH(aq) = acetic acid
(c) McGraw Hill Ryerson 2007

9. BASES Bases can be gentle or very caustic. Examples of common bases:
NaOH(aq)
Mg(OH)2(aq)
Ca(OH)2(aq)
NH4OH(aq)
See page 227
(c) McGraw Hill Ryerson 2007

10. everyday acids laboratory acids
What is an acid?
Acids are a group of chemicals.
everyday acids
laboratory acids
Can you think of other examples of acids?

11. What is a weak acid? Strong acids cannot be touched and are corrosive.
Weak acids are safe to handle and have a sour taste.

12. everyday bases laboratory bases
What is a base?
Bases are another group of chemicals, the opposite of acids.
everyday bases
laboratory bases
Can you think of other examples of bases?

13. What is a weak base?
Bases are used for cleaning. Strong bases are caustic and cause redness on the skin.
Weak bases are soapy and safe to touch.

14. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 What is the pH scale? stronger acid
The strength of an acid or base is measured by the pH scale.
Each universal indicator colour is given a number called the pH value.
Universal indicator can tell you the pH of a solution.
stronger acid
stronger base
strongacid
weakacid
weak base
strongbase
neutral

15. What is an indicator? Litmus is red in acid. Litmus is blue in base.
How can you test a liquid to find if it is an acid or an base?
An indicator is a special chemical that changes
to a different colour in an acid or an base.
Litmus paper and litmus solution are examples of indicators.
Litmus is red in acid.
Litmus is
blue in base.

16. Litmus test experiment
The results for the litmus tests are:
Tube 1. The solution is an alkali which turns blue when red litmus is added to it and remains blue when blue litmus is added to it.
Tube 2. The solution is an acid which remains red when red litmus is added to it and turns blue when red litmus is added to it.
Tube 3. The solution is water which remains red when red litmus is added to it and remains blue when blue litmus is added to it.

17. What type of substance? 7 Are these substances acidic or basic?
Are they weak or strong?
Substance pH
Description of acid/base
soda water 6
car battery acid 1
soap 8
washing soda 10
stomach acid 2
oven cleaner 14
vinegar 4
very weak acid
very strong acid
very weak base
weak base
strong acid
very strong base
weak acid
base
acid 1 2 14 13 12 11 10 9 8 7 6 5 4 3

18. General Reaction: #3: Metals with Acid acid salt hydrogen metal MgCl2
Example:
MgCl2
HCl Mg H2

19. #3: Metals with Acid

20. Some Properties of Acids
Produce H3O+ (as H3O+) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule)
Taste sour
Corrode metals
Electrolytes
React with bases to form a salt and water
pH is less than 7
Turns blue litmus paper to red “Blue to Red A-CID”

21. Some Properties of Bases
Produce OH- ions in water
Taste bitter, chalky
Are electrolytes
Feel soapy, slippery
React with acids to form salts and water
pH greater than 7
Turns red litmus paper to blue “Basic Blue”

22. All acids, bases and salts dissolve in water.
Summary Chart
Property
Acid
Base
Salt
Definition
produce H+
produce OH-
ionic compound
Example
HCl, CH3COOH
NaOH, NH3
NaCl pH
1-2, 3-6
8 – 11, 12 – 14 7
red litmus
red
blue
stays red
blue litmus
stays blue
Universal indicator
red – yellow
ROY
blue – violet
BIV
green G
taste sour
vinegar,
lemon juice
corrosive
feel soapy
household cleaners
caustic
All acids, bases and salts dissolve in water.

23. Some Common Bases NaOH sodium hydroxide lye
KOH potassium hydroxide liquid soap
Ba(OH)2 barium hydroxide stabilizer for plastics
Mg(OH)2 magnesium hydroxide “MOM” Milk of magnesia
Al(OH)3 aluminum hydroxide Maalox (antacid)

24. Why can bicarbonate of soda (pH 9) be used to treat a bee sting?
Neutralizing stings
A bee sting
is acidic.
A wasp sting
is alkaline.
Why can bicarbonate of soda (pH 9) be used to treat a bee sting?
Why can vinegar (pH 3)
be used to treat
a wasp sting?

25. Observations NaOH(aq) HCl(aq) Taste Bitter Sour
*Usually, but not always
NaOH(aq)
HCl(aq)
Taste
Bitter
Sour
Feel (choose slippery or not slippery)
Slippery
Not slippery
pH (# from the key) 14 1
Litmus (blue or red)
Blue
Red
Phenolphthalein
*Pink
*Cloudy/ white
Bromothymol
*Blue
*Yellow
Magnesium NR
Bubbles
Baking soda NR
Bubbles

26. See page 229
(c) McGraw Hill Ryerson 2007

27. Acid: is any substance that releases H+ in water
Old Idea
Arrhenius Theory
Acid: is any substance that releases H+ in water
Base: is any substance that releases OH- in water

28. Arrhenius acid
Chemistry 11
produces H+ in solution
HCl 
H Cl-
Arrhenius base
Chemistry 11
produces OH- in solution
NaOH  Na OH-

29. Arrhenius acid is a substance that produces H3O+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water

30. Acid: is any substance that donates H+ to other substance
New Idea
Bronsted Theory
Acid: is any substance that donates H+ to other substance
Base: is any substance that accepts H+ from other substances

31. New Idea
Bronsted Theory
Give
Acid H+
Take
Base

32. New Idea
Bronsted Theory
Hydrogen is given and taken

33. New Idea Bronsted Theory Hydrogen is given and taken
How many electron, proton and neutron does it have?
Electron
Proton
Neutron

34. New Idea Bronsted Theory Hydrogen is given and taken
How many electron, proton and neutron does it have?
Electron
Proton
Neutron 1

35. How does Hydrogen ion look like?
New Idea
Bronsted Theory
Hydrogen is given and taken
This is Hydrogen Atom
How does Hydrogen ion look like?

36. How many electron, proton and neutron does it have?
New Idea
Bronsted Theory
Hydrogen is given and taken
This is Hydrogen Atom
How many electron, proton and neutron does it have?

37. New Idea Bronsted Theory Hydrogen is given and taken Electron Proton
Neutron 1

38. Suggest a name of Hydrogen Ion?
New Idea
Bronsted Theory
Suggest a name of Hydrogen Ion?
Electron
Proton
Neutron 1

39. Hydrogen ion aka proton Suggest a name of Hydrogen Ion?
New Idea
Bronsted Theory
Hydrogen ion aka proton
Suggest a name of Hydrogen Ion?
Electron
Proton
Neutron 1

40. Bronsted Acid
Chemistry 12
A proton donor H+
HCl H2O 
H3O Cl-
Bronsted Base
Chemistry 12
A proton acceptor
NH H2O ⇄
NH OH- H+

42. Note
1. Arrhenius bases dissociate in water to produce OH-
2. Bronsted bases accept a proton from water to produce OH-
3. Arrhenius acids dissociate in water to form H+
4. Bronsted acids donate a proton to water to form H3O+
5. H+ is the same as H3O+

43. H+ is another way to show H3O+.
H H2O ⇋
H3O+
Hydronium ion + H+
H2O

44. Conjugate
acid base pairs differ by one proton H+

45. Conjugate Acid
Conjugate Base
One more H+
1 less H+
C6H5OH
C6H5O-
H2CO3
HCO3-
H2O
OH-
HPO42-
PO43-
H2PO4-
HPO42-
C6H5COOH
C6H5COO-
NH4+
NH3
Fe(H2O)63+
Fe(H2O)5(OH)2+

46. Examples: Conj Acid-Base Pairs
HCl NO2-1
NH3
HCN
HSO4-1
CO3-2
For conj, acid:
add an H+
For conj., base:
remove H+
Chapter

48. Practice problems
Identify the acid, base, conjugate acid, conjugate base, and conjugate acid-base pairs:
HC2H3O2(aq) + H2O(l)  C2H3O2–(aq) + H3O+(aq)
acid
base
conjugate base
conjugate acid
conjugate acid-base pairs
OH –(aq) + HCO3–(aq)  CO32–(aq) + H2O(l)
base
acid
conjugate base
conjugate acid
conjugate acid-base pairs

49. Answers: question 18 (a) HF(aq) + SO32–(aq)  F–(aq) + HSO3–(aq) acid
base
conjugate base
conjugate acid
conjugate acid-base pairs
(b)
CO32–(aq) + HC2H3O2(aq)  C2H3O2–(aq) + HCO3–(aq)
base
acid
conjugate base
conjugate acid
(c)
conjugate acid-base pairs
H3PO4(aq) + OCl –(aq)  H2PO4–(aq) + HOCl(aq)
acid
base
conjugate base
conjugate acid
conjugate acid-base pairs

50. HCO3–(aq) + S2–(aq)  HS–(aq) + CO32–(aq) acid base conjugate acid
conjugate base
conjugate acid-base pairs
8b)
H2CO3(aq) + OH –(aq)  HCO3–(aq) + H2O(l)
acid
base
conjugate base
conjugate acid
conjugate acid-base pairs
11a)
H3O+(aq) + HSO3–(aq)  H2O(l) + H2SO3(aq)
acid
base
conjugate base
conjugate acid
conjugate acid-base pairs
11b)
OH –(aq) + HSO3–(aq)  H2O(l) + SO32–(aq)
base
acid
conjugate acid
conjugate base
conjugate acid-base pairs
For more lessons, visit

51. Tutorial 14 Questions

52. protics
monoprotic
Polyprotics
Diprotic
Triprotics
Amphiprotics

53. ------ protics Monoprotic: give one proton
Polyprotic: give more than proton
Diprotic give two protons
Triporotic give three protons

54. Different types of acids can ionize to release one or more protons
A monoprotic acid releases a single proton when it ionizes (e.g. hydrochloric acid):
A diprotic acid can release two protons when it ionizes (e.g. sulfuric acid):
For sulfuric acid, the first ionization is complete (as indicated by the single arrow), therefore it is a strong electrolyte

55. A triprotic Acid can release three protons when it ionizes(e. g
A triprotic Acid can release three protons when it ionizes(e.g. phosphoric acid)
H3PO4(aq) H+(aq) + H2PO4- (aq)
H2PO4- (aq) H+(aq) + HPO42-(aq)
HPO42-(aq) H+(aq) + PO43-(aq)

56. Polyprotics Give protons in many small steps H3PO4+H2OH2PO41-+H3O+
HPO42- +H2O PO43- +H3O+

57. ------ protics Polyprotic: Give protons in many small steps
H3PO4H2PO41-  HPO42-  PO43-

58. Amphiprotic Can be acid and base like HCO3- Can give or take proton
protics
Amphiprotic Can be acid and base like HCO3- Can give or take proton

59. ------ protics Amphiprotic Can be acid and base like HCO3-
Can give or take proton
H3PO4H2PO41-  HPO42-  PO43-

60. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43-

61. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43- Base can gain H+, cannot lose H+
HPO42-

62. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43- Base can gain H+, cannot lose H+
HPO42- Amphiprotic can gain H+and lose H+
H2PO4-

63. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43- Base can gain H+, cannot lose H+
HPO42- Amphiprotic can gain H+and lose H+
H2PO4- Amphiprotic can gain H+and lose H+
H3PO4

64. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43- Base can gain H+, cannot lose H+
HPO42- Amphiprotic can gain H+and lose H+
H2PO4- Amphiprotic can gain H+and lose H+
H3PO4 Acid cannot gain H+, can lose H+

65. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO32-

66. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO Base
HCO3-

67. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO Base
HCO3- Amphiprotic
H2CO3

68. Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO Base
HCO3- Amphiprotic
H2CO3 Acid

69. Tutorial 14 Questions

70. Properties and uses of the acids and bases
Topic 4.2
Properties and uses of the acids and bases
Page
Worksheet 4.1