Transcript Chapter 9 Acids and Bases
Chapter 9 Acids and Bases
Ionization of Water The pH Scale
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Ionization of Water
Occasionally, in water, a H + is transferred between H 2 O molecules H : . . . . . . . .
O . .
: + : O : H . .
H : O : H + . . + : O : H . .
H H H water molecules hydronium hydroxide ion (+) ion (-)
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Pure Water is Neutral
Pure water contains small, but equal amounts of ions: H 3 O + and OH H 2 O + H H 3 O + OH 2 O H 3 O + + OH hydronium hydroxide ion ion 1 x 10 -7 M 1 x 10 -7 M
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Ion Product of Water K
w [ ] = Molar concentration K w = [ H 3 O + ] [ OH ] = [ 1 x 10 -7 ][ 1 x 10 -7 ] = 1 x 10 -14
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Acids
Increase H +
HCl (g) + H 2 O (l) H 3 O + (aq) + Cl (aq)
More [H 3 O + ] than water > 1 x 10 -7 M
As H 3 O + increases, OH decreases [H 3 O + ] > [OH ] H 3 O + OH -
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Bases
Increase the hydroxide ions (OH )
NaOH (s) H 2 O Na + (aq) + OH (aq)
More [OH ] than water, [OH ] > 1 x 10 -7 M
When OH increases, H 3 O + decreases [OH
] > [H 3 O + ] OH H 3 O +
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Using K
w The [OH ] of a solution is 1.0 x 10 - 3 M. What is the [H 3 O + ]?
K w = [H 3 O + ] [OH ] = 1.0 x 10 -14 [H 3 O + ] = 1.0 x 10 -14 [OH ] [H 3 O + ] = 1.0 x 10 -14 1.0 x 10 - 3
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= 1.0 x 10 -11 M
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Learning Check pH1
The [H 3 O + ] of lemon juice is 1.0 x 10 -3 What is the [OH ] of the solution?
M. 1) 1.0 x 10 3 M 2) 3) 1.0 x 10 -11 M 1.0 x 10 11 M
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Solution pH1
The [H 3 O + ] of lemon juice is 1.0 x 10 - 3 M. What is the [OH ]?
[OH ] = 1.0 x 10 -14 1.0 x 10 - 3 = 1.0 x 10 -11 M
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Using the Calculator
1.0 x 10 -14 4.0 x 10 -5 Enter 1.0
EE +/ 14
4.0
EE +/ 5 = 2.5 x 10 -10
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Learning Check pH2
The [OH-] of a solution is 5 x 10 -5 M. What is the [H 3 O + ] of the solution?
1) 2) 3) 2 x 10 - 5 M 1 x 10 10 M 2 x 10 -10 M
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Solution pH2
The [OH ] of a water solution is 5 x 10 -5 M. What is the [H 3 O + ] in the solution?
[ H 3 O + ] = 1.0 x 10 -14 5 x 10 - 5 On some calculators: 1.0
EE +/ 14
5 EE +/ 5 = 2 x 10 -10 M
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Learning Check pH3
A.The [OH ] when [H 3 O + ] of 1 x 10 - 4 M 1) 1 x 10 -6 M 2) 1 x 10 -8 M 3) 1 x 10 -10 M B.The [H 3 O + ] when [OH ] of 5 x 10 -9 M 1) 1 x 10 - 6 M 2) 2 x 10 - 6 M 3) 2 x 10 -7 M
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Solution pH3
K w = [H 3 O + ][OH ] = 1.0 x 10 14 A. (3) [OH ] = 1.0 x 10 -14 = 1.0 x 10 1.0 x 10 - 4 -10 B.
(2) [H 3 O + ] = 1.0 x 10 -14 = 2 x 10 - 6 5 x 10 - 9
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pH
Indicates the acidity [H 3 O + ] of the solution
pH = - log [H 3 O + ]
From the French pouvoir hydrogene
(“hydrogen power” or power of hydrogen)
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pH
In the expression for [H 3 O + ] 1 x 10 -exponent the exponent = pH
[H
3
O
+
] = 1 x 10
pH
M
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pH Range
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Acidic Basic [H + ] > [OH ] Neutral [H + ] = [OH ]
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[OH ] >
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[H + ]
Some [H
3
O
+
] and pH
[H 3 O + ]
1 x 10
5
M 1 x 10
9
M 1 x 10
11
M
pH 5 9 11
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pH of Some Common Acids gastric juice lemon juice vinegar orange juice coffee milk 1.0
2.3
2.8
3.5
5.0
6.6
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pH of Some Common Bases blood tears seawater milk of magnesia household ammonia 7.4
7.4
8.4
10.6
11.0
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Learning Check pH4
A. The [H 3 O + ] of tomato juice is 1 x 10 -4 M. What is the pH of the solution?
1) - 4 2) 4 3) 8 B. The [OH ] of an ammonia solution is 1 x 10 -3 M. What is the pH of the solution?
1) 3 2) 11 3) -11
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Solution pH4
A. pH = - log [ 1 x 10 -4 ] = -(- 4) = 4 B. [H 3 O + ] = 1 x 10 -11 pH = - log [ 1 x 10 - 11 ] = -(- 11) = 11
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Learning Check pH5
The pH of a soap is 10. What is the [H 3 O + ] of the soap solution?
1) 1 x 10 - 4 M 2) 1 x 10 10 M 3) 1 x 10 - 10 M
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Solution pH5
The pH of a soap is 10. What is the [H 3 O + ] of the soap solution?
[H 3 O + ] = 1 x 10 pH M = 1 x 10 10 M
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pH on the Calculator
[H 3 O + ] is 4.5 x 10 -6 M pH = 4.5 x EXP(or EE) 6+/ LOG +/ = 5.35
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Learning Check pH6
A soap solution has a [H 3 O + ] = 2 x 10 -8 M. What is the pH of the solution? 1) 8 2) 7.7
3) 6
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Solution pH6
A soap solution has a [H 3 O + ] = 2.0 x 10 -8 M. What is the pH of the solution? B) 2.0 EE 8 +/ LOG +/- = 7.7
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Learning Check pH7
Identify each solution as 1. acidic 2. basic A. _____ HCl with a pH = 1.5 3. neutral B. _____ Pancreatic fluid [H + ] = 1 x 10 -8 M C. _____ Sprite soft drink pH = 3.0
D. _____ pH = 7.0
E. _____ [OH ] = 3 x 10 -10 M F. _____ [H + ] = 5 x 10 -12
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Solution pH7
Identify each solution as 1. acidic 2. basic A. _1__ HCl with a pH = 1.5 B. _2__ 3. neutral Pancreatic fluid [H + ] = 1 x 10 -8 M C. _1__ D. _3__ E. _1__ F. _2__ Sprite soft drink pH = 3.0
pH = 7.0
[OH ] = 3 x 10 -10 M [H + ] = 5 x 10 -12
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Acid Rain
Unpolluted rain has a pH of 5.6
Rain with a pH below 5.6 is “acid rain“
CO 2 in the air forms carbonic acid CO 2 + H 2 O
Adds to H + of rain H 2 CO 3 H 2 CO 3 H + (aq) + HCO 3 -(aq)
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Sources of Acid Rain
Power stations
Oil refineries
Coal with high S content
Car and truck emissions
Bacterial decomposition, and lighting hitting N 2
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SO 2 NO and NO 2 Mt. St Helens (1980) 26 million tons in 1980 22 million tons in 1980 400,000 tons SO 2
Reactions with oxygen in air form SO 3 2SO 2 + O 2 2 SO 3
Reactions with water in air form acids SO 3 + H 2 O NO + H 2 O H 2 SO 4 sulfuric acid HNO 2 nitrous acid HNO 2 + H 2 O HNO 3 nitric acid
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Effects of Acid Rain
Leaches Al from soil, which kills fish
Fish kills in spring from runoff due to accumulation of large amounts of acid in snow
Dissolves waxy coatings that protect leaves from bacteria
Corrodes metals, textiles, paper and leather
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