1. CHAPTER 19
ACID, BASES & SALTS
Open Textbook to page 586

2. MANY SUBSTANCES CONTAIN ACIDS.
VINEGAR (ACETIC ACID)
CARBONATED DRINKS (PHOSPHORIC ACID)
GRAPE JUICE (TARTARIC ACID)
APPLES (MALIC ACID)
LEMONS (CITRIC ACID)

3. MANY SUBSTANCES CONTAIN BASES.
LYE (SODIUM HYDROXIDE) FOUND IN
COMMERCIAL DRAIN CLEANERS
MILK OF MAGNESIA (MAGNESIUM HYDROXIDE)
BAKING SODA (SODIUM BICARBONATE)

5. ACIDS: 5 GENERAL PROPERTIES: HAVE A SOUR TASTE.
CHANGE THE COLOR OF ACID-BASE
INDICATORS.
REACT WITH ACTIVE METALS
TO RELEASE H2 (g).
Mg (s) HCl (aq)  MgCl2 + H2 (g)

6. REACT WITH BASES TO PRODUCE
SALTS AND WATER.
5) SOME ACIDS CONDUCT ELECTRIC CURRENT.

7. ACID NOMENCLATURE
BINARY ACID:
ACID THAT CONTAINS ONLY
2 DIFFERENT ELEMENTS,
i.e.,
HYDROGEN AND ONE OF THE MORE
ELECTRONEGATIVE ELEMENTS.

8. NAMES OF BINARY ACIDS HF HYDROFLUORIC ACID HCl HYDROCHLORIC ACID
HBr HYDROBROMIC ACID
HI HYDROIODIC ACID
H2S HYDROSULFURIC ACID

9. OXYACIDS ACID THAT IS A COMPOUND OF HYDROGEN, OXYGEN, AND
a 3rd ELEMENT USUALLY A
NONMETAL

10. COMMON OXYACIDS CH3COOH Acetic acid H2CO3 Carbonic acid
HNO3 Nitric acid
H3PO4 phosphoric acid
H2SO4 sulfuric acid
H2SO3 sulfurous acid
HClO4 perchloric acid
HClO3 chloric acid
HClO2 chlorous acid
HClO hypochlorous acid

11. Common Industrial Acids
SULFURIC ACID:
MOST COMMONLY PRODUCED INDUSTRIAL CHEMICAL
USED IN CAR BATTERIES

12. NITRIC ACID:
STAINS PROTEINS YELLOW
USED IN MAKING EXPLOSIVES

13. PHOSPHORIC ACID:
USED DIRECTLY FOR MANUFACTURING
FERTILIZERS AND ANIMAL FEED.
FLAVORING AGENT IN SOFT DRINKS

14. HYDROCHLORIC ACID:
PRODUCED BY STOMACH
IN HARDWARE STORES, DILUTE SOL’N KNOWN
AS MURIATIC ACID AND IS USED TO CORRECT
ACIDITY OF SWIMMING POOLS AND TO
CLEAN MASONRY.

15. BASES 5 GENERAL PROPERTIES
TASTE BITTER.
CHANGE THE COLOR OF ACID-BASE INDICATORS.
DILUTE AQUEOUS SOLUTIONS FEEL SLIPPERY.

16. BASES 5 GENERAL PROPERTIES
REACT WITH ACIDS TO PRODUCE SALTS AND WATER.
CONDUCT ELECTRIC CURRENT.

17. Svante Arrhenius
Theory limited
to aqueous
solutions

18. ARRENHIUS ACIDS & BASES
INCREASES THE CONC.
OF HYDROGEN IONS, H+, IN AQUEOUS SOLUTIONS

19. ARRENHIUS ACIDS & BASES
ARRENHIUS BASE:
INCREASES THE CONCENTRATION
OF HYDROXIDE IONS, OH-, IN AQUEOUS SOLUTIONS

20. AQUEOUS SOLUTIONS OF BASES
ALKALINE
IONIC HYDROXIDES WHICH DISSOCIATE IN SOLUTION TO RELEASE OH- (aq).
SODIUM HYDROXIDE: NaOH
NaOH (s)  Na+ (aq) + OH- (aq)

21. Group 1 Hydroxides
NaOH
KOH
LiOH
RbOH
CsOH
Group 2 Hydroxides
Ca(OH)2
Ba(OH)2
Sr(OH)2

22. Another ACID-BASE THEORIES
ARRENHIUS DEFINITION REQUIRES SUBSTANCES TO BE AQUEOUS.
DEFINITIONS REVISED TO INCLUDE SUBSTANCES WHEN THEY ARE NOT IN A WATER SOLUTION.

23. BRONSTED-LOWRY ACIDS & BASES
A MOLECULE or ION THAT IS A
PROTON DONOR.
HCl + NH3  NH Cl-
HCl transfers a proton to the ammonia molecule

24. Figure 14.3 The Reaction of NH3 with HCl to Form NH4+ and Cl-

25. BRONSTED-LOWRY BASE
MOLECULE OR ION THAT IS A PROTON ACCEPTOR.

26. The Reaction of NH3 with HCl to Form NH4+ and Cl- AMMONIA ACCEPTS A PROTON FROM HCl thus AMMONIA IS A BRONSTED-LOWRY BASE

27. BONSTED-LOWRY ACID-BASE REACTION
PROTONS ARE TRANSFERRED FROM ONE REACTANT (THE ACID)
TO ANOTHER (THE BASE).

28. ACID-BASE REACTIONS BRONSTED-LOWRY ACID DONATES A H+
SPECIES REMAINING COULD RE-ACCEPT THAT H+ AND THUS ACT AS A BASE

29. CONJUGATE BASE
SPECIES THAT REMAINS AFTER A BRONSTED-LOWRY ACID HAS GIVEN UP A H+ ION.
HF (aq) + H2O (l)  F- (aq) + H3O+ (aq)
acid conjugate
base

30. BRONSTED-LOWRY BASE ACCEPTS A H+
SPECIES REMAINING COULD RE-DONATE THAT H+ AND THUS ACT AS AN ACID

31. CONJUGATE ACID
SPECIES THAT FORMS AFTER A BRONSTED-LOWRY BASE HAS ACCEPTED A H+ ION.
HF (aq) + H2O (l)  F- (aq) + H3O+ (aq)
base conjugate
acid

32. Are equilibrium systems meaning that both the
BRONSTED-LOWRY
ACID-BASE REACTIONS
Are equilibrium systems meaning that both the
Forward and the reverse reactions occur.
Each contain two conjugate acid-base pairs.

33. Let’s identify the Conjugate Acid-Base Pairs
HNO3 (l) + H2O (l)  H3O+ (aq) + NO3- (aq)

34. Conjugate Acid/Base Pairs
HA(aq) + H2O(l)  H3O+(aq) + A(aq)
conj conj conj conj
acid base acid base 1
DO PROBLEM 48 on page 625

35. AMPHOTERIC COMPOUNDS
SPECIES THAT CAN ACT AS EITHER AN ACID OR A BASE
H2SO4(aq) + H2O  H3O+(aq) + HSO4- (aq)
base
NH3 (g) + H2O (l)  NH4+(aq) + OH- (aq)
acid

36. Water as an Acid and a Base
Water is amphoteric (it can behave either as an acid or a base).
H2O (l) + H2O(l)  H3O+ + OH
conj conj
acid base acid base 1

37. MONOPROTIC ACIDS
ACIDS THAT CAN DONATE ONLY ONE HYDROGEN ION PER MOLECULE.
EXAMPLES
HCl
HNO3
HClO4

38. Polyprotic Acids
. . . can furnish more than one Hydrogen ion (H+) to the solution.
Examples:
H2SO4
H3PO4

39. All polyprotic acids ionize in a stepwise
Manner i.e., one HYDROGEN ION
at a time.
H2SO4 (l) + H2O (l)  H3O+ (aq) + HSO4- (aq)
HSO4- (aq) + H2O (l)  H3O+ (aq) + SO42- (aq)
Each step is weaker than the one before; therefore,
concentration of ions formed in the first step is the
greatest.

40. POLYPROTIC ACIDS DIPROTIC ACID:
CAN DONATE TWO HYDROGEN IONS PER MOLECULES.
TRIPROTIC ACID:
CAN DONATE THREE
HYDROGEN IONS
PER MOLECULE

41. Lewis Acids and Bases Emphasizes role of electron pairs to form a covalent bond
Lewis Acid: electron pair acceptor
Lewis Base: electron pair donor

42. The Al(H2O)63+ ion

43. Aluminum ion (Lewis Acid) accepts electron pairs
From Water (Lewis Base) donates electron pairs
to form covalent bonds.
Lewis Acid-Base Reaction:
formation of one or more covalent bonds
between an electron-pair donor and an electron-pair
acceptor.

44. LEWIS DEFINITION BROADEST OF THE
THREE ACID-BASE DEFINITIONS

45. STRONG ACIDS
ACID THAT IONIZES COMPLETELY IN AQUEOUS SOLUTION.

46. STRONG ACID Solutions MEMORIZE!!! HClO4 (aq) H2SO4 (aq) HNO3 (aq)
HCl (aq)
HBr (aq)
HI (aq)
MEMORIZE!!!

47. WEAK ACIDS ACID THAT IONIZES LESS THAN COMPLETELY IN AQUEOUS SOLUTION.
. Ka is the acid dissociation constant.
Smaller the Ka the weaker the acid.

48. Figure 14.4 Graphic Representation of the Behavior of Acids of Different Strengths in Aqueous Solution a) Strong Acid b) Weak Acid

49. Figure 14.6 A Strong Acid (a) and a Weak Acid (b) in Water

50. NaOH(s)  Na+(aq) + OH(aq)
Bases
“Strong” and “weak” are used in the same sense for bases as for acids.
strong = complete dissociation (hydroxide ion supplied to solution)
NaOH(s)  Na+(aq) + OH(aq)

51. Strong Bases (Strong electrolytes)
Group 1A Hydroxides
NaOH
KOH
LiOH
RbOH
CsOH
Group 2A Hydroxides
Ca(OH)2
Ba(OH)2
Sr(OH)2

52. WEAK BASES
(Weak electrolytes):
Weak = incomplete dissociation
Kb is the base dissociation constant.
Smaller the Kb the weaker the base.
NH ammonia
CH3NH2 methylamine
Other organic compounds that contain
nitrogen atoms.