1. Chapter 20 Acids and Bases

2. Section 20.1 Describing Acids and Bases
OBJECTIVES:
List the properties of acids and bases.

3. Section 20.1 Describing Acids and Bases
OBJECTIVES:
Name an acid or base, when given the formula.

4. Properties of acids Taste sour (don’t try this at home).
Conduct electricity.
Some are strong, others are weak electrolytes.
React with metals to form hydrogen gas.
Change indicators (blue litmus to red).
React with hydroxides to form water and a salt.

5. Properties of bases React with acids to form water and a salt.
Taste bitter.
Feel slippery (don’t try this either).
Can be strong or weak electrolytes.
Change indicators (red litmus turns blue).

6. Names and Formulas of Acids
An acid is a chemical that produces hydrogen ions (H1+) when dissolved in water
Thus, general formula = HA, where A is a monatomic or polyatomic anion
HCl(g) is hydrogen monochloride
HCl(aq) is named as an acid
Name focuses on the anion present

7. Names and Formulas of Acids
1. BINARY - When anion ends with -ide, the acid starts with hydro-, and the stem of the anion has the suffix -ic followed by the word acid
2. TERNARY - When anion ends with -ite, the anion has the suffix -ous, then acid
3. TERNARY - When anion ends with -ate, the anion suffix is -ic and then acid

8. Names and Formulas of Bases
A base produces hydroxide ions (OH1-) when dissolved in water.
Named the same way as any other ionic compound
name the cation, followed by anion
To write the formula: write symbols; write charges; then cross (if needed)
Sample Problem 20-1, p. 579

9. Section 20.2 Hydrogen Ions and Acidity
OBJECTIVES:
Given the hydrogen-ion or hydroxide-ion concentration, classify a solution as neutral, acidic, or basic.

10. Section 20.2 Hydrogen Ions and Acidity
OBJECTIVES:
Convert hydrogen-ion concentrations into values of pH, and hydroxide-ion concentrations into values of pOH.

11. Hydrogen Ions from Water
Water ionizes, or falls apart into ions:
H2O ® H1+ + OH1-
Called the “self ionization” of water
Occurs to a very small extent:
[H1+ ] = [OH1-] = 1 x 10-7 M
Since they are equal, a neutral solution results from water
Kw = [H1+ ] x [OH1-] = 1 x 10-14
Kw is called the “ion product constant”

12. Ion Product Constant H2O H+ + OH-
Kw is constant in every aqueous solution: [H+] x [OH-] = 1 x 10-14
If [H+] > 10-7 then [OH-] < 10-7
If [H+] < 10-7 then [OH-] > 10-7
If we know one, other can be determined
If [H+] > 10-7 , it is acidic and [OH-] < 10-7
If [H+] < 10-7 , it is basic and [OH-] > 10-7
Basic solutions also called “alkaline”
Sample problem 20-2, p. 582

13. Logarithms and the pH concept
Logarithms are powers of ten.
Review from earlier lessons, and p. 585
definition: pH = -log[H+]
in neutral pH = -log(1 x 10-7) = 7
in acidic solution [H+] > 10-7
pH < -log(10-7)
pH < 7 (from 0 to 7 is the acid range)
in base, pH > 7 (7 to 14 is base range)

14. pH and pOH pH = -log[H+] pOH = -log [OH-]
Kw = [H+] x [OH-] = 1 x 10-14
pH + pOH = 14
Thus, a solution with a pH less than 7 is an acid; a pH greater than 7 is a base; 7 is neutral

15. [H+]
100
10-1
10-3
10-5
10-7
10-9
10-11
10-13
10-14 pH 1 3 5 7 9 11 13 14
Acidic
Neutral
Basic 1 3 5 7 9 11 13 14
pOH
Basic
100
10-1
10-3
10-5
10-7
10-9
10-11
10-13
10-14
[OH-]

16. Examples: Sample 20-3, p.586 Sample 20-4, p.586 Sample 20-5, p.587

17. Measuring pH Why measure pH?
Everything from swimming pools, soil conditions for plants, medical diagnosis, soaps and shampoos, etc.
Sometimes we can use indicators, other times we might need a pH meter

18. Acid-Base Indicators
An indicator is an acid or base that undergoes dissociation in a known pH range, and has different colors in solution (more later in chapter)
Examples: litmus, phenolphthalein, bromthymol blue: Fig 20.8, p.590

19. Acid-Base Indicators
Although useful, there are limitations to indicators:
usually given for a certain temperature (25 oC), thus may change at different temperatures
what if the solution already has color?
ability of human eye to distinguish colors

20. Acid-Base Indicators A pH meter may give more definitive results
some are large, others portable
works by measuring the voltage between two electrodes
needs to be calibrated
Fig , p.591

21. Section 20.3 Acid-Base Theories
OBJECTIVES:
Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis

22. Section 20.3 Acid-Base Theories
OBJECTIVES:
Identify conjugate acid-base pairs in acid-base reactions.

23. Svante Arrhenius
Swedish chemist ( ) - Nobel prize winner in chemistry (1903)
one of the first chemists to explain the chemical theory of the behavior of acids and bases
Dr. Hubert Alyea-last graduate student of Arrhenius. (link below)

24. Svante Arrhenius ( )

25. Hubert N. Alyea ( )

26. 1. Arrhenius Definition
Acids produce hydrogen ions (H1+) in aqueous solution.
Bases produce hydroxide ions (OH1-) when dissolved in water.
Limited to aqueous solutions.
Only one kind of base (hydroxides)
NH3 (ammonia) could not be an Arrhenius base.

27. Polyprotic Acids Some compounds have more than 1 ionizable hydrogen.
HNO3 nitric acid - monoprotic
H2SO4 sulfuric acid - diprotic - 2 H+
H3PO4 phosphoric acid - triprotic - 3 H+
Having more than one ionizable hydrogen does not mean stronger!

28. Polyprotic Acids
However, not all compounds that have hydrogen are acids
Also, not all the hydrogen in an acid may be released as ions
only those that have very polar bonds are ionizable - this is when the hydrogen is joined to a very electronegative element

29. Arrhenius examples... Consider HCl What about CH4 (methane)?
CH3COOH (ethanoic acid, or acetic acid) - it has 4 hydrogens like methane does…?
Table 20.4, p. 595 for bases

30. 2. Brønsted-Lowry Definitions
Broader definition than Arrhenius
Acid is hydrogen-ion donor (H+ or proton); base is hydrogen-ion acceptor.
Acids and bases always come in pairs.
HCl is an acid.
When it dissolves in water, it gives it’s proton to water.
HCl(g) + H2O(l) H3O+ + Cl-
Water is a base; makes hydronium ion.

31. Johannes Bronsted / Thomas Lowry (1879-1947) (1874-1936)

32. Acids and bases come in pairs...
A conjugate base is the remainder of the original acid, after it donates it’s hydrogen ion
A conjugate acid is the particle formed when the original base gains a hydrogen ion
Indicators are weak acids or bases that have a different color from their original acid and base

33. Acids and bases come in pairs...
General equation is:
HA(aq) + H2O(l) H3O+(aq) + A-(aq)
Acid + Base Conjugate acid Conjugate base
NH3 + H2O NH41+ + OH1-
base acid c.a c.b.
HCl + H2O H3O1+ + Cl1-
acid base c.a c.b.
Amphoteric - acts as acid or base

34. 3. Lewis Acids and Bases
Gilbert Lewis focused on the donation or acceptance of a pair of electrons during a reaction
Lewis Acid - electron pair acceptor
Lewis Base - electron pair donor
Most general of all 3 definitions; acids don’t even need hydrogen!
Sample Problem 20-7, p.599

35. Gilbert Lewis ( )

36. Section 20.4 Strengths of Acids and Bases
OBJECTIVES:
Define strong acids and weak acids.

37. Section 20.4 Strengths of Acids and Bases
OBJECTIVES:
Calculate an acid dissociation constant (Ka) from concentration and pH measurements.

38. Section 20.4 Strengths of Acids and Bases
OBJECTIVES:
Arrange acids by strength according to their acid dissociation constants (Ka).

39. Section 20.4 Strengths of Acids and Bases
OBJECTIVES:
Arrange bases by strength according to their base dissociation constants (Kb).

40. Strength Strong acids and bases are strong electrolytes
They fall apart (ionize) completely.
Weak acids don’t completely ionize.
Strength different from concentration
Strong-forms many ions when dissolved
Mg(OH)2 is a strong base- it falls completely apart when dissolved.
But, not much dissolves- not concentrated

41. Measuring strength Ionization is reversible. HA H+ + A-
This makes an equilibrium
Acid dissociation constant = Ka
Ka = [H+ ][A- ] (water is constant) [HA]
Stronger acid = more products (ions), thus a larger Ka (Table 20.8, p.602)

42. What about bases? Strong bases dissociate completely.
B + H2O BH+ + OH-
Base dissociation constant = Kb
Kb = [BH+ ][OH-] [B] (we ignore the water)
Stronger base = more dissociated, thus a larger Kb.

43. Strength vs. Concentration
The words concentrated and dilute tell how much of an acid or base is dissolved in solution - refers to the number of moles of acid or base in a given volume
The words strong and weak refer to the extent of ionization of an acid or base
Is concentrated weak acid possible?

44. Practice Write the expression for HNO2 Write the Kb for NH3
Sample 20-8, p. 604
Carefully study Key Terms and equations, p. 608
Be sure to do the ChemASAP programs, and take all the self-tests that are available!