chapter 16 acids and bases ionization of water the ph scale 7-4
TRANSCRIPT
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Chapter 16Acids and Bases
Ionization of Water
The pH Scale
7-4
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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
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pH of Some Common Acids
gastric juice 1.0
lemon juice 2.3
vinegar 2.8
orange juice 3.5
coffee 5.0
milk 6.6
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pH of Some Common Bases
blood 7.4
tears 7.4
seawater 8.4
milk of magnesia 10.6
household ammonia 11.0
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Calculating pH, pOHpH = -log10 [H3O+]
pOH = -log10 [OH-]
Relationship between pH and Relationship between pH and pOHpOH pH + pOH = 14
Finding [HFinding [H33OO++], [OH], [OH--] from pH, pOH] from pH, pOH
[H3O+] = 10-pH
[OH-] = 10-pOH
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In pure water, [H3O+] = [OH-] = 1 10 –7 Kw = 1 10 –14
pH pOH
[H+] [OH-]
pH + pOH = 14
pOH = -log[OH-]pH = -log[H+]
[H+][OH-] = 1.0 10-14
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pH +
pOH = 14
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Ionization of Water
Occasionally, in water, a H+ is transferred between H2O 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: H3O+ and OH-
H2O + H2O H3O+ + OH-
hydronium hydroxide
ion ion
1 x 10-7 M 1 x 10-7 MH3O+ OH-
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Ion Product of Water Kw
[ ] = Molar concentration
Kw = [ H3O+ ] [ OH- ]
= [ 1 x 10-7 ][ 1 x 10-7 ]
= 1 x 10-14
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Acids
Increase H+
HCl (g) + H2O (l) H3O+ (aq) + Cl-
(aq)
More [H3O+] than water > 1 x 10-7M
As H3O+ increases, OH- decreases
[H3O+] > [OH-]
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Bases
Increase the hydroxide ions (OH-) H2O
NaOH (s) Na+(aq) + OH- (aq)
More [OH-] than water, [OH-] > 1 x 10-7M
When OH- increases, H3O+ decreases
[OH] > [H3O+]
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Using Kw
The [OH- ] of a solution is 1.0 x 10- 3 M. What is the
[H3O+]?
Kw = [H3O+ ] [OH- ] = 1.0 x 10-14
[H3O+] = 1.0 x 10-14
[OH-]
[H3O+] = 1.0 x 10-14 = 1.0 x 10-11 M
1.0 x 10- 3
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Learning Check pH
The [H3O+] of lemon juice is 3.0 x 10-3 M. What
is the [OH-] of the solution?
Kw = [H3O+ ] [OH- ] = 1.0 x 10-14
[OH- ] = 1.0 x 10-14
[H3O+]
[OH- ] = 1.0 x 10-14 = 3.3 x 10-12 M
3.0 x 10- 3
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pH
The [H3O+] of lemon juice is 9.0 x 10- 4 M.
What is the [OH-]?
[OH- ] = 1.0 x 10 -14 = 1.1 x 10-11 M 9.0 x 10 - 4
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The [H3O+] is 4.0 x 10- 5 M. What is the [OH-]?
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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Solution pH
B.The [H3O+] when [OH- ] of 5 x 10-9 M
Kw = [H3O+ ][OH-] = 1.0 x 10 14
[H3O+] = 1.0 x 10 -14 = 2 x 10 - 6
5 x 10- 9
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pH
Indicates the acidity [H3O+] of the solution
pH = - log [H3O+]
From the French pouvoir hydrogene
(“hydrogen power” or power of
hydrogen)
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In the expression for [H3O+]
1 x 10-exponent
the exponent = pH
[H3O+] = 1 x 10-pH M
pH
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pH Range
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
Neutral
[H+]>[OH-] [H+] = [OH-] [OH-]>[H+]
Acidic Basic
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pH
A. The [H3O+] of tomato juice is 1 x 10-4 M. What is the pH of the solution?
answer: 4
pH = - log [ 1 x 10-4] = -(- 4) = 4
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pH
B. The [OH-] of an ammonia solution is
1 x 10-3 M. What is the pH of the solution?
Answer: 11
[H3O+] = 1 x 10-11
pH = - log [ 1 x 10- 11] = -(- 11) = 11
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Some [H3O+] and pH
[H3O+] pH
1 x 10-5 M 5
1 x 10-9 M 9
1 x 10-11 M 11
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Solution pH
The pH of a soap is 10. What is the [H3O+]
of the soap solution?
[H3O+] = 1 x 10-pH M
= 1 x 10-10 M
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pH on the Calculator
[H3O+] is 4.5 x 10-6 M. What is the pH.
pH = 4.5 x EXP(or EE) 6+/- LOG +/-
= 5.35
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Learning Check pH
A soap solution has a [H3O+] = 2 x 10-8 M.
What is the pH of the solution?
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pH
A soap solution has a [H3O+] = 2.0 x 10-8
M. What is the pH of the solution?
2.0 EE 8 +/- LOG +/- = 7.7
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Learning Check
Identify each solution as
1. acidic 2. basic 3. neutral
A. _____ HCl with a pH = 1.5
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
1
2
1
3
1
2
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What is the [H3O+ ] or [OH- ] in each of the following solutions, also state if the solution is neutral, acidic, or basic.a. 1 10 -5 M OH- b. 1 10 -7 M OH- c. 10.0 M H+
a. 1.0 x 10-9 Mb. 1.0 x 10-7 Mc. 1.0 x 10-15 M
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