1. Acids
Lesson 2
Acid and Base
Properties

2. Properties of Acids
Neutralize bases
Are electrolytes that conduct electricity
React with metals such as Mg and Zn to make H2
Change litmus paper red
Taste sour
Properties of Bases
Neutralize acids
Feel slippery
Change litmus paper blue
Taste bitter

3. Arrhenius acid (Chemistry 11):  

4. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.

5. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-

6. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11):  

7. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.

8. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-

9. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12):

10. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor

11. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor
HCl + H2O 

12. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor
HCl + H2O  H+

13. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor
HCl + H2O  H3O Cl- H+

14. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor
HCl + H2O  H3O Cl-
Bronsted Base (Chemistry 12): A proton acceptor

15. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor
HCl + H2O  H3O Cl-
Bronsted Base (Chemistry 12): A proton acceptor
NH H2O ⇄ H+

16. Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
HCl  H Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
NaOH  Na OH-
Bronsted Acid (Chemistry 12): A proton donor
HCl + H2O  H3O Cl-
Bronsted Base (Chemistry 12): A proton acceptor
NH H2O ⇄ NH OH- H+

17. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄

18. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄
base acid H+

19. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH- H+

20. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH-
base acid H+

21. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH-
Base acid H+ H+

22. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH-
Base acid acid base H+ H+

23. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH-
Base acid acid base
Conjugate acid base pairs differ by one proton H+

24. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH-
Base acid acid base
Conjugate acid base pairs differ by one proton
HCO3- and H2CO3

25. Complete the Bronsted reaction assuming HCO3- is a base.
HCO H2O ⇄ H2CO OH-
Base acid acid base
Conjugate acid base pairs differ by one proton
HCO3- and H2CO3 H2O and OH-

26. 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. This leads us to the conclusion that H+ is the same as H3O+.

27. H+ is another way to show H3O+. We can treat them as the same
H+ is another way to show H3O+. We can treat them as the same. H+ is really just a proton.
H H2O +

28. H+ is another way to show H3O+. We can treat them as the same
H+ is another way to show H3O+. We can treat them as the same. H+ is really just a proton.
H H2O
proton water +

29. H+ is another way to show H3O+. We can treat them as the same
H+ is another way to show H3O+. We can treat them as the same. H+ is really just a proton.
H3O+ +

30. + This is called the hydronium ion
H+ is another way to show H3O+. We can treat them as the same. H+ is really just a proton.
H3O+
This is called the hydronium ion +

31. Conjugate Acid Conjugate Base
One more H less H+
NH  

32. Conjugate Acid Conjugate Base
One more H less H+
NH NH3
H2O

33. Conjugate Acid Conjugate Base
One more H less H+
NH NH3
H3O+ H2O
H2O

34. Conjugate Acid Conjugate Base
One more H less H+
NH NH3
H3O+ H2O
H2O OH-
HCO3-

35. Conjugate Acid Conjugate Base
One more H less H+
NH NH3
H3O+ H2O
H2O OH-
H2CO3 HCO3-
H2PO4-

36. Conjugate Acid Conjugate Base
One more H less H+
NH NH3
H3O+ H2O
H2O OH-
H2CO3 HCO3-
H2PO4- HPO42-
PO43-

37. Conjugate Acid Conjugate Base
One more H less H+
NH NH3
H3O+ H2O
H2O OH-
H2CO3 HCO3-
H2PO4- HPO42-
HPO PO43-

38. Conjugate Acid Conjugate Base
CH3COOH

39. Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COO-

40. Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH

41. Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O-
CO32-

42. Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O-
HCO CO32-
HPO42-

43. Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O-
HCO CO32-
HPO PO43-
HO2-

44. Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O-
HCO CO32-
HPO PO43-
H2O2 HO2-

45. Strong Acids
There are six on the top of the Acid Chart- p6.
All completely ionize in water.
All are very good conductors.
All produce lots of H3O+.
All have very large Ka.
Use a “” and not “⇄”
HCl + H2O

46. Strong Acids
There are six on the top of the Acid Chart- p6.
All completely ionize in water.
All are very good conductors.
All produce lots of H3O+.
All have very large Ka.
Use a “” and not “⇄”
HCl + H2O  H3O Cl-

47. Weak Acids
Left side of the Acid Chart below the top six.
Partially ionize in water.
Are poor conductors.
Produce small amounts of H3O+.
Have small Ka’s.
Use a “⇄” and not “”
HF + H2O

48. Weak Acids
Left side of the Acid Chart below the top six.
Do not completely ionize in water.
Are poor conductors.
Produce small amounts of H3O+.
Have small Ka’s.
Use a “⇄” and not “”
HF + H2O ⇄ H3O F-

49. Weak Acids
Left side of the Acid Chart below the top six.
Do not completely ionize in water.
Are poor conductors.
Produce small amounts of H3O+.
Have small Ka’s.
Use a “⇄” and not “”
HF + H2O ⇄ H3O F-
Ka = [H3O+][F-]
= 3.5 x from page 6
[HF]
Water is not included because it is a pure liquid!
Its concentration is constant!

50. You can also write:
HF ⇌ H F-
Ka = [H+][F-]
= 3.5 x 10-4
[HF]

51. Writing Ionic Equations: Formula, Complete, and Net.
HCl NaOH  NaCl + H2O(l)
H Cl Na OH-  Na Cl H2O(l)
H OH-  H2O(l)
Do not break up weak acids or bases!
HF KOH  KF + H2O(l)
HF K OH-  K F H2O(l)
HF OH-  F H2O(l)