chapter 18 acid base equilibria - linn-benton community...
TRANSCRIPT
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Chapter 18
Acid Base Equilibria
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Properties of Acids and Bases
Acids Bases
Release H+ Release OH-
Neutralize OH- Neutralize H+
Proton Donors Proton Acceptors
Electron Pair Acceptors Electron Pair Donors
pH < 7 pH > 7
Taste Sour Taste Bitter, Feel Slippery
Litmus Paper (turns pink) Litmus paper (turns blue)
Reacts with most metals
to form H2(g)
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Neutralization Reaction
Acid + Base Salt + H2O(l)
Strong acids and bases dissociate approximately
100%
Strong Acids: HCl, HBr, HI, HNO3, HClO4, HClO3,
H2SO4
Strong Bases: Soluble metal hydroxides
Weak acids and bases dissociate << 100%
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Fig.
18.1
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Weak Acid Equilibrium Expression
HA H+ + A-
Ka = [H+][A-] or
[HA]
Ka = [H3O+][A-]
[HA]
HA + H2O(l) H3O+ + A-
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Fig.
18.2
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Example
Write the equilibrium expression for the following
dissociation of benzoic acid:
Note: A 2 M solution only dissociates about 0.6%
O
O H
O
O
+ H
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Fig.
18.3
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Weak Base Characteristics
Weak bases, such as insoluble metal
hydroxides, dissociate << 100% in water---
releasing few OH- ions.
Weak bases, such as ammonia, amines and
amides, slightly react with water to release
OH- ions. This process is also called
dissociation.
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Weak Base Equilibrium Expression
Kb = [HB+][OH-]
[B]
B + H2O(l) HB+ + OH-
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Example
Write the equilibrium expression for the following
dissociation:
NH3 + H2O(l) NH4+ + OH-
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Autoionization of Water
Water self-ionizes. Pure water dissociates, but very
little. It is a very weak electrolyte.
Write equilibrium expressions for the following
dissociations:
H2O(l) + H2O(l) H3O+ + OH-
H2O(l)H+ + OH-
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Autoionization of Water Cont.
Using your equilibrium table/problem solving
technique learned in the last chapter,
determine the [H+] and [OH-] in water.
Kw = 1.0 X 10-14
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Fig.
18.4:
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Problem Solving
1. If HNO3 is added to H2O, the [H3O+] is
2.0 X 10-5M, what is the [OH-]?
2. If LiOH is added to water, the [OH-] is 2.0 X 10-5 M, what is the [H+]?
3. If H+ is added to water in which direction will the equilibrium shift?
4. If OH- is added to water in which direction will the equilibrium shift?
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pH
The following relationships are often used to determine the pH and pOH of a solution.
pH = - log [H+] pOH = - log [OH-]
pKw = -log Kw 14 = pH + pOH
If the pH = 7, the solution is neutral; [H+] = [OH-]
If the pH < 7, the solution is acidic; [H+] > [OH-]
If the pH > 7, the solution is basic; [H+] < [OH-]
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Fig. 18.5
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Fig.
18.6
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Fig. 18.7
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Problem Solving
Determine the pH, pOH, [H+], [OH-] as appropriate for the following problems.
a. A sample of blood has a pH of 7.40.
b. A household ammonia solution has a [OH-]=7.94X10-3 M.
c. A sample of rain water has a pH of 5.40.
d. A 0.0400 M HBr solution.
e. A 0.0250 M NaOH solution.
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More Problem Solving
1. What is the pH, pOH, [H+], [OH-] of a 0.20 M
Ba(OH)2 solution?
2. Consider a 3.00 L 0.00100 M HCl solution.
If 50.0 mL of 0.00900 M NaOH is added,
what is the pH of the solution?
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Bronsted-Lowry Acids and Bases
Recall: Acids are proton donors and bases are
proton acceptors.
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Fig.
18.8
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An acid-base conjugate pair: Two species of an
acid-base reaction that differ by the loss or gain of a
proton (H+).
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Application Time!
Look at the following acid-base reactions and
determine (a) the acid, (b) the base, and (c)
the acid-base conjugate pairs in each.
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CO32- + H2O(l) HCO3
- + OH-
C2H3O2- + HNO2 HC2H3O2 + NO2
-
HCO3- + H2O(l) H3O+ + CO3
2-
HCO3- + H2O(l) OH- + H2CO3
Note: A substance that can act as an acid or a base is said to be amphiprotic.
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Fig. 18.9: Strength relationship between acid-base conjugate pairs.
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Lewis Acids and Bases
Recall: An acid can also be an electron pair
acceptor and a base can be an electron pair
donor.
Example: See the next slide
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Label the Lewis acid and base. The product is
called an adduct.
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Acid-Base Pair Strength Relationships
The higher the Ka, the stronger the acid, the
weaker the conjugate base.
Note: pKa = -log Ka
The higher the Ka, the lower the pKa.
The stronger the acid, the weaker the
conjugate base.
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Weak Monoprotic Acid Problem
Solving
1. Determine the equilibrium constant for a 0.10 M phenol (HC6H5O) solution that has a pH of 5.43 at 250C. What is the degree of ionization of this weak acid?
2. What are the concentrations of nicotinic acid, hydogen ion, and nicotinate ion in a solution of 0.15 M nicotinic acid (HC6H4O2) at 25oC? What is the pH? What is the percent ionization?
Ka = 1.4 x 10-5
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3. Determine the percent ionization for each of the
following solutions: 0.10 M HC2H3O2 and 0.0010
M HC2H3O2. Ka = 1.7 x 10-5
4. When 5.00 grains of aspirin are dissolved in 0.500
liters of solution, 0.325 grams of acetylsalicylic
acid (HC9H7O4) are present. What is the pH of the
solution?
Ka = 3.3 x 10-4
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Polyprotic Acids
Polyprotic Acids are compounds that contain
more than one acidic hydrogen.
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General Equilibrium Expressions for a
Triprotic Acid
H3A H+ + H2A- Ka1 =[H+][H2A-]
[H3A]
H2A- H+ + HA2- Ka2 =[H+][HA2-]
[H2A-]
HA2- H+ + A3- Ka3 =[HA2-]
[H+][A3-]
Note: Ka3 < Ka2 < Ka1 Why?
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Problem Solving for Polyprotic Acids
1. Tartaric Acid, H2C4H4O6 is a diprotic acid.
What is the pH of a 0.10 M solution? What
is the concentration of C4H4O62-?
Ka1 = 9.2 x 10-4 and Ka2 = 4.3 x 10-5
2. What is the pH of a 0.10 M ascorbic acid
(H2Asc) solution?
Ka1 = 7.9 x 10-5 and Ka2 = 1.6 x 10-12
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Weak Base Equilibria
Relationships worth knowing:
Kw = KaKb for weak acid-base conjugate pairs.
Write equilibrium expressions for each of the following
reactions and prove the above statement.
HB H+ + B-
B- + H2O HB + OH-
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Weak bases include amines and amides such as
the following molecule.
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Conjugate Base of a Weak Acid
The conjugate base (anion) of a weak acid can
react with water. Write a general reaction and
the equilibrium expression for this process.
Would you use Ka or Kb?
If given Ka how would you determine Kb?
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Problem Solving for Weak Base
1. Determine Kb of a 6.0 M weak base having a
pH of 12.02.
2. Dissolved aniline, C6H5NH2, is used in
perfumes. What is the pH of a 0.035 M
solution?
Kb = 4.2 x 10-10
A- + H2O HA + OH-
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Acid-Base Properties of Salt Solutions
Hydrolysis of an ion with water can produce an acidic or basic solution.
Examples: Determine if the aqueous solutions below are acidic, basic, or neutral.
Ammonium chloride
Ammonium cyanide
Iron(III) nitrate
Sodium chloride
Ammonium hypochlorite
Aluminum chloride
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Problem Solving
1. What is the pH of a 0.10 M sodium acetate
solution? pKa = 4.74
2. If 3.00 g of KClO are added to 100 mL of
water, what is the pH of the solution.
Ka = 2.9 x 10-8