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Chapter 9 Acids and Bases Ionization of Water The pH Scale

LecturePLUS Timberlake

1

Ionization of Water Occasionally, in water, a H+ is transferred between H2O molecules

..

..

..

H:O: +

:.O.:H

H:O:H +

.. H

H

water molecules

..

.. +

:O : H..

H hydronium hydroxide ion (+) ion (-) LecturePLUS Timberlake

2

Pure Water is Neutral Pure water contains small, but equal amounts of ions: H3O+ and OH-

H2O + H2O H 3O +

OH-

H3O+

+

OH-

hydronium hydroxide ion ion

1 x 10-7 M 1 x 10-7 M LecturePLUS Timberlake

3

Ion Product of Water Kw [ Kw

] = Molar concentration =

[ H3O+ ] [ OH- ]

=

[ 1 x 10-7 ][ 1 x 10-7 ]

=

1 x 10-14 LecturePLUS Timberlake

4

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-] LecturePLUS Timberlake

H 3O +

OH5

Bases Increase the hydroxide ions (OH-) H2 O

NaOH (s) Na+(aq) + OH- (aq) More [OH-] than water, [OH-] > 1 x 10-7M  When OH- increases, H3O+ decreases [OH− ] > [H3O+] LecturePLUS Timberlake

H 3O +

OH6

Using Kw The [OH- ] of a solution is 1.0 x 10- 3 M. What is the [H3O+]? Kw

=

[H3O+ ] [OH- ]

[H3O+]

=

1.0 x 10-14

= 1.0 x 10-14

[OH-] [H3O+] =

1.0 x 10-14 1.0LecturePLUS x 10- 3Timberlake

= 1.0 x 10-11 M 7

Learning Check pH1 The [H3O+] of lemon juice is 1.0 x 10-3 M. What is the [OH-] of the solution? 1)

1.0 x 103 M

2)

1.0 x 10-11 M

3)

1.0 x 1011 M LecturePLUS Timberlake

8

Solution pH1 The [H3O+] 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

=

LecturePLUS Timberlake

1.0 x 10-11 M

9

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

LecturePLUS Timberlake

10

Learning Check pH2 The [OH-] of a solution is 5 x 10 -5 M. What is the [H3O+ ] of the solution? 1)

2 x 10- 5 M

2)

1 x 1010 M

3)

2 x 10-10 M LecturePLUS Timberlake

11

Solution pH2 The [OH-] of a water solution is 5 x 10-5 M. What is the [H3O+] in the solution? [ H3O+] = 1.0 x 10 -14 5 x 10- 5 On some calculators: 1.0 EE +/- 14

÷ 5 EE +/- 5 = 2 x 10 -10 M LecturePLUS Timberlake

12

Learning Check pH3 A.The [OH-] when [H3O+ ] 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 [H3O+] 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 LecturePLUS Timberlake

13

Solution pH3 Kw = [H3O+ ][OH-] = 1.0 x 10 14 A. (3) [OH- ] =

1.0 x 10 -14 = 1.0 x 10 -10 1.0 x 10- 4

B. (2) [H3O+] =

1.0 x 10 -14 = 2 x 10 - 6 5 x 10- 9 LecturePLUS Timberlake

14

pH  Indicates the acidity [H3O+] of the solution  pH = - log [H3O+]  From the French pouvoir hydrogene (“hydrogen power” or power of hydrogen)

LecturePLUS Timberlake

15

pH In the expression for [H3O+]

1 x 10-exponent the exponent = pH

[H3O+] = 1 x 10-pH M LecturePLUS Timberlake

16

pH Range 0

1

2

3 4 5

6

7 8 9 10 11 12 13 14 Basic

Acidic

Neutral

[H+]>[OH ] -

[H+] = [OH-] LecturePLUS Timberlake

[OH-]>[H ] +

17

Some [H3O+] and pH [H3O+]

pH

1 x 10-5 M

5

1 x 10-9 M

9

1 x 10-11 M

11

LecturePLUS Timberlake

18

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 LecturePLUS Timberlake

19

pH of Some Common Bases blood

7.4

tears

7.4

seawater

8.4

milk of magnesia

10.6

household ammonia

11.0

LecturePLUS Timberlake

20

Learning Check pH4 A. The [H3O+] 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 LecturePLUS Timberlake

3)

-11 21

Solution pH4 A. pH = - log [ 1 x 10-4] = -(- 4) = 4 B. [H3O+] = 1 x 10-11 pH = - log [ 1 x 10- 11] = -(- 11) = 11

LecturePLUS Timberlake

22

Learning Check pH5 The pH of a soap is 10. What is the [H3O+] of the soap solution? 1) 1 x 10 - 4 M 2) 1 x 1010 M 3) 1 x 10 - 10 M LecturePLUS Timberlake

23

Solution pH5 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 LecturePLUS Timberlake

24

pH on the Calculator [H3O+] is 4.5 x 10-6 M pH = 4.5 x EXP(or EE) 6+/- LOG +/= 5.35

LecturePLUS Timberlake

25

Learning Check pH6 A soap solution has a [H3O+] = 2 x 10-8 M. What is the pH of the solution? 1) 8 2) 7.7 3) 6 LecturePLUS Timberlake

26

Solution pH6 A soap solution has a [H3O+] = 2.0 x 10-8 M. What is the pH of the solution?

B) 2.0

EE

8

+/-

LOG +/- = 7.7

LecturePLUS Timberlake

27

Learning Check pH7 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 LecturePLUS Timberlake

28

Solution pH7 Identify each solution as 1. acidic 2. basic

3. neutral

A. _1__

HCl with a pH = 1.5

B. _2__

Pancreatic fluid [H+] = 1 x 10-8 M

C. _1__

Sprite soft drink pH = 3.0

D. _3__

pH = 7.0

E. _1__

[OH-] = 3 x 10-10 M

F. _2__

[H+] = 5 x 10-12 LecturePLUS Timberlake

29

Acid Rain Unpolluted rain has a pH of 5.6 Rain with a pH below 5.6 is “acid rain“ CO2 in the air forms carbonic acid CO2 + H2O

H2CO3

Adds to H+ of rain H2CO3

H+ (aq) + HCO3-(aq) LecturePLUS Timberlake

30

Sources of Acid Rain Power stations Oil refineries Coal with high S content Car and truck emissions Bacterial decomposition, and lighting hitting N2 LecturePLUS Timberlake

31

SO2

26 million tons in 1980

NO and NO2

22 million tons in 1980

Mt. St Helens (1980)

400,000 tons SO2

Reactions with oxygen in air form SO3 2SO2 + O2

2 SO3

Reactions with water in air form acids SO3 + H2O

H2SO4 sulfuric acid

NO + H2O

HNO2 nitrous acid

HNO2 + H2O

HNO nitric acid

LecturePLUS Timberlake 3

32

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 LecturePLUS Timberlake

33

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