1. Acids and Bases

2. Properties of Acids and Bases
Acids: taste sour, react with metals to produce hydrogen gas, conduct electricity.
Bases: taste bitter, feel slippery, conduct electricity.

3. Definitions of Acids and Bases
Arrhenius definition
Acid- produces hydrogen ions in aqueous solution
Base- produces hydroxide ions in aqueous solution
This definition is limited only to aqueous solutions and allows for only one kind of base.

4. Definitions of Acids and Bases
Bronsted-Lowrey definition
Acid- proton (H+) donor
Base-proton acceptor
This is a more general definition
Under this definition, water can act as both an acid and a base and is said to be amphoteric.
When water acts as a base and accepts a proton, the hydronium ion (H3O+) is formed.

5. Definitions of Acids and Bases
Lewis Acid-Base model
acid-electron pair acceptor (has an
empty orbital that can be used to
share an electron pair
base-electron pair donor (has a lone
pair of electrons)
Covers many reactions not covered by the other definitions.
Example: BF3 + NH3  F3BNH3
Lewis Lewis
acid base

6. Formation of Acids/Bases
General reaction when an acid is dissolved in water:
HA + H2O  H3O+ + A-
acid base conjugate conjugate
acid base
Conjugate base- remains of the acid particle after the proton has been donated.
Conjugate acid- is formed when the proton is transferred to the base.

7. Application of Equilibrium
The equation representing the formation of conjugate acids/bases really represents a competition for the proton between the two bases, H2O and A-.
If H2O is a much stronger base (has a stronger affinity for the proton) than A-, the equilibrium position lies far to the right. (Most of the acid will be in the ionized form).
If A- is a much stronger base than H2O, the equilibrium position will lie far to the left. (Most of the acid will be present as HA).

8. Acid Dissociation Constant
The equilibrium constant for the dissociation of an acid is called the acid dissociation constant (Ka).
Because H2O does not appear in the equilibrium expression (pure liquid), it is often not included in the equation.
If water is not included in the equation, H3O+ will be represented simply as H+.

9. Acid Strength
Strong acid- almost completely ionized; equilibrium lies far to the right/ a strong acid produces a weak conjugate base (much weaker than water).
Weak acid- dissociates only to a small extent; equilibrium lies far to the left/ a weak acid produces a strong conjugate base (much stronger than water).

10. Autoionization of Water
Because water is amphoteric, water can transfer a proton from one water molecule to another to produce a hydronium ion and a hydroxide ion.
2 H2O (l) <---> H3O+ (aq) + OH- (aq)
Kw = [H3O+][OH-]
Kw is the dissociation constant for water

11. Dissociation Constant for Water
Experiments show that at 25oC,
[H3O+] = [OH-] = 1x10-7 M
Therefore, at 25oC
Kw = [H3O+][OH-] = (1x10-7)(1x10-7)
= 1x10-14

12. The Significance of Kw
In any aqueous solution at 25oC, no matter what it contains, the product of [H3O+] and [OH-] must always equal
1x There are three possible situations:
1. A neutral solution, where [H3O+] = [OH-]
2. An acidic solution, where [H3O+] > [OH-]
3. A basic solution, where [H3O+] < [OH-]

13. Sample Problems
Calculate the [H3O+] and [OH-] for each of the following and state whether the solution is acidic, basic, or neutral.
a) 1.0 x 10-5 M OH-
b) 1.0 x 10-7 M OH-
c) 10.0 M H30+

14. Sample Problem At 60oC, the value of Kw is 1x10-13.
a) Using LeChatelier’s Principle, predict
whether the reaction:
2H20 < -- > H3O+ + OH-
is exothermic or endothermic.
b) Calculate [H3O+] and [OH-] in a neutral
solution at 600C.

15. The pH Scale
Because [H3O+] is typically very small, the pH scale provides a convenient way to represent solution acidity.
pH = -log[H3O+]
For a solution where [H3O+] = 1.0 x 10-7 M,
pH = 7.00
Rules for significant digits: the number of decimal places in the log is equal to the number of significant digits in the original number.

16. Similar log scales
Similar log scales are used for representing other quantities:
pOH = -log[OH-]
pK = -logK
**** pH + pOH = 14.00

17. Polyprotic Acids Polyprotic acids can supply more than one proton.
Examples include: H2SO4, H3PO4, etc.
Polyprotic acids always dissociate in a step wise manner, one proton at a time.
Ka1 > Ka2> Ka3 and this is generally true for all inorganic acids.
Successive ionization constants often decrease by a factor of 104 to 106.
This means that each step in the ionization of a polyprotic acid occurs to a much lesser extent than the previous step.

18. Acid-Base Properties of Salts
Salt is another name for an ionic compound.
When a salt is dissolved in water, it breaks up into ions.
Under certain conditions, these ions can behave as acids or bases.

19. Salts that Produce Neutral Solutions
Salts that consist of the cations of strong bases and the anions of strong acids have no effect on the [H+] when dissolved in water.
This means that aqueous solutions of salts such as KCl, NaCl, NaNO3, and KNO3 are neutral (pH=7).

20. Which salt will be neutral (pH =7)?10
NaC2H3O2
KCN
FeCl3
NaNO3 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

21. Which salt will be neutral?10
KCl
NaF
KNO2
Li3PO4 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

22. Which salt will be neutral?10
KClO
NH4ClO2
KClO3
NH4ClO4 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

23. Salts that Produce Basic Solutions
For any salt whose cation has neutral properties (such as Na+ or K+) and whose anion is the conjugate base of a weak acid, the aqueous solution will be basic.
The Kb value for the ion can be obtained from the relationship Kb = Kw/Ka.

24. Example of a Basic Salt
NaC2H3O2 completely ionizes in water to form Na+ and C2H3O2- ions.
Na+ ions have no affinity for H+ ions and cannot produce H+ so they have no effect on the pH
C2H3O2- ions are the conjugate base of a weak acid and have a significant affinity for protons, therefore acting as a base.
C2H3O2- + H2O < -- > HC2H3O2 + OH-
A base reacts with water to produce hydroxide ions and a conjugate acid.

25. Which of the following salts is basic (pH>7)?10
KNO3
KCN
K2SO4
KCl 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

26. Which salt is basic? FeCl3 NaNO2 NH4ClO3 Al2(SO4)3 10 1 2 3 4 5 6 7 89 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

27. Which salt is basic? NaClO KNO3 FeSO4 LiBr 10 1 2 3 4 5 6 7 8 9 10 1112 13 14 15 16 17 18 19 20 21 22 23 24 25 26

28. Salts that Produce Acidic Solutions
Salts in which the anion is not a base (from a strong acid) and the cation is the conjugate acid of a weak base produce acidic solutions.
The Ka value for the ion can be obtained from the relationship Ka = Kw / Kb
A second type of salt that produces an acidic solution is one that contains a highly charged metal ion (ex. Al(H2O)63+)
Typically, the higher charge on the metal ion, the stronger the acidity of the hydrated ion.

29. Example of an Acidic Salt
NH4Cl completely ionizes in water to form NH4+ and Cl- ions.
Cl- ions have no affinity for protons and does not affect the pH.
NH4+ ions are the conjugate acid of a weak base and therefore act as an acid.
NH H2O < -- > NH3 + H3O+
An acid reacts with water to produce hydronium ions and a conjugate base.

30. Which salt is acidic (pH<7)?10
NaNO3
NaC2H3O2
NH4Cl
KCN 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

31. Which salt is acidic? KNO2 KNO3 NaCN NH4ClO3 10 1 2 3 4 5 6 7 8 9 1011 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

32. Which salt is acidic? CH3NH3Cl KF RbBr NaSO3 10 1 2 3 4 5 6 7 8 9 1011 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26

33. Salts in Which Both Ions Have Acidic or Basic Properties
Salts, such as NH4C2H3O2, consist of two ions that can both affect the pH of the solution (both are ions of weak acids/bases).
We will only consider the qualitative nature of these situations.
A prediction can be made about whether the solution will be acidic, basic, or neutral by comparing the Ka value of the acidic ion with the Kb value of the basic ion.
If Kb > Ka, the solution will be basic.
If Ka > Kb, the solution will be acidic.
If Ka = Kb, the solution will be neutral.

34. KNO3 is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1617 18 19 20 21 22 23 24 25 26

35. NaNO2 is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 1516 17 18 19 20 21 22 23 24 25 26

36. C5H5NHClO4 is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 1415 16 17 18 19 20 21 22 23 24 25 26

37. NH4NO2 is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 1516 17 18 19 20 21 22 23 24 25 26

38. KClO is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1617 18 19 20 21 22 23 24 25 26

39. NH4ClO is Acidic Basic Neutral 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1617 18 19 20 21 22 23 24 25 26

40. KCl is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1617 18 19 20 21 22 23 24 25 26

41. NH4C2H3O2 is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 1415 16 17 18 19 20 21 22 23 24 25 26

42. CH3NH3Cl is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 1415 16 17 18 19 20 21 22 23 24 25 26

43. KF is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1617 18 19 20 21 22 23 24 25 26

44. NH4F is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1617 18 19 20 21 22 23 24 25 26

45. CH3NH3CN is Acidic Basic Neutral 10 1 2 3 4 5 6 7 8 9 10 11 12 13 1415 16 17 18 19 20 21 22 23 24 25 26

46. An unknown salt is either NaCN, NH4Cl, NH4C2H3O2, or NaOCl3. When 0
An unknown salt is either NaCN, NH4Cl, NH4C2H3O2, or NaOCl3. When mole of the salt is dissolved in 1.0 L of solution, the pH is > 7. What is the identity of the salt? 10
NaCN
NH4Cl
NH4C2H3O2
NaClO3 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26