fundamentals of analytical chemistry 9th edition pdf

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The pH ranges shown are approximate.
Specific transition ranges depend on the
indicator solvent chosen.

Reprinted by permission of the Hach Company

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Unless otherwise noted, all content on this page is © Cengage Learning.

PERIODIC TABLE OF THE ELEMENTS
Metals

IA
1

Metalloids

1

1

2

3

4

5

6

7

VIIA
17

Nonmetals

0
18

1

2

IIIA
13

IVA
14

VA
15

VIA

16

H

He

1.008

IIA
2

1.008

4.0026

3

4

5

6

7

8

9

10

Li

Be

B

C

N

O

F

Ne

6.941

9.0122

10.81

12.011

14.007

15.999

18.9984

20.1797

H

11

12

Na

Mg

22.9898

13

14

15

16

17

18

IIB
12

Al

Si

P

S

Cl

Ar

10

IB
11

26.9815

28.085

30.9738

32.06

35.453

39.948

27

28

29

30

31

32

33

34

35

36

Fe

Co

Ni

Cu

Zn

Ga

Ge

As

Se

Br

Kr

55.845

58.9332

58.6934

63.546

65.38

69.723

72.63

74.9216

78.96

79.904

83.798

VIIIB

24.3050

IIIB
3

IVB
4

VB
5

VIB
6

VIIB
7

8

9

19

20

21

22

23

24

25

26

K

Ca

Sc

Ti

V

Cr

Mn

39.0983

40.078

44.9559

47.867

50.9415

51.9961

54.9380

37

38

39

40

41

42

43

44

45

46

47

48

49

50

51

52

53

54

Rb

Sr

Y

Zr

Nb

Mo

Tc

Ru

Rh

Pd

Ag

Cd

In

Sn

Sb

Te

I

Xe

85.4678

87.62

88.9058

91.224

92.9064

95.96

(98)

101.07

102.9055

106.42

107.8682

112.411

114.818

118.710

121.760

127.60

126.9045

131.293

55

56

57

Cs

Ba

La

72

73

74

75

76

77

78

79

80

81

82

83

84

85

86

Hf

Ta

W

Re

Os

Ir

Pt

Au

Hg

Tl

Pb

Bi

Po

At

Rn

132.9055

137.327

87

88

138.9055

178.49

180.9479

183.84

186.207

190.23

192.217

195.084

196.9666

200.59

204.38

207.2

208.9804

(209)

(210)

(222)

89

104

105

106

107

108

109

110

111

112

113

114

115

116

117

Fr

Ra

Ac

118

Rf

Db

Sg

Bh

Hs

Mt

Ds

Rg

Cn

Uut

Fl

Uup

Lv

Uus

Uuo

(223)

(226)

(227)

(265)

(268)

(271)

(270)

(277)

(276)

(281)

(280)

(285)

(284)

(289)

(288)

(293)

(294)

(294)

*

**

*Lanthanide Series

Note: Atomic masses are 2009
IUPAC values (up to four decimal
places). More accurate values for
some elements are given in the
table inside the back cover.

58

59

60

61

62

63

64

65

66

67

68

69

70

71

Ce

Pr

Nd

Pm

Sm

Eu

Gd

Tb

Dy

Ho

Er

Tm

Yb

Lu

140.116

140.9076

144.242

(145)

150.36

151.964

157.25

158.9254

162.500

164.9303

167.259

168.9342

173.054

174.9668

** Actinide Series
90

91

92

93

94

95

96

97

98

99

100

101

102

103

Th

Pa

U

Np

Pu

Am

Cm

Bk

Cf

Es

Fm

Md

No

Lr

(237)

(244)

(243)

(247)

(247)

(251)

(252)

(257)

(258)

(259)

(262)

232.0381 231.0359 238.0289

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International Atomic Masses

Element

Actinium
Aluminum
Americium
Antimony
Argon
Arsenic
Astatine
Barium
Berkelium
Beryllium
Bismuth
Bohrium
Boron
Bromine
Cadmium
Calcium
Californium
Carbon
Cerium
Cesium
Chlorine
Chromium

Cobalt
Copernicium
Copper
Curium
Darmstadtium
Dubnium
Dysprosium
Einsteinium
Erbium
Europium
Fermium
Flerovium
Fluorine
Francium
Gadolinium
Gallium
Germanium
Gold
Hafnium
Hassium
Helium
Holmium
Hydrogen
Indium
Iodine
Iridium
Iron
Krypton
Lanthanum
Lawrencium

Lead
Lithium
Livermorium
Lutetium
Magnesium
Manganese
Meitnerium


Symbol

Atomic
Number

Atomic
Mass

Ac
Al
Am
Sb
Ar
As
At
Ba
Bk
Be
Bi
Bh
B

Br
Cd
Ca
Cf
C
Ce
Cs
Cl
Cr
Co
Cn
Cu
Cm
Ds
Db
Dy
Es
Er
Eu
Fm
Fl
F
Fr
Gd
Ga
Ge
Au
Hf
Hs
He

Ho
H
In
I
Ir
Fe
Kr
La
Lr
Pb
Li
Lv
Lu
Mg
Mn
Mt

89
13
95
51
18
33
85
56
97
4
83
107
5

35
48
20
98
6
58
55
17
24
27
112
29
96
110
105
66
99
68
63
100
114
9
87
64
31
32
79
72
108
2

67
1
49
53
77
26
36
57
103
82
3
116
71
12
25
109

(227)
26.9815386
(243)
121.760
39.948
74.92160
(210)
137.327
(247)
9.012182
208.98040
(270)
10.81

79.904
112.411
40.078
(251)
12.011
140.116
132.90545
35.45
51.9961
58.933195
(285)
63.546
(247)
(281)
(268)
162.500
(252)
167.259
151.964
(257)
(289)
18.9984032
(223)
157.25
69.723
72.63
196.966569
178.49
(277)
4.002602

164.93032
1.008
114.818
126.90447
192.217
55.845
83.798
138.90547
(262)
207.2
6.94
(293)
174.9668
24.3050
54.938045
(276)


Element

Mendelevium
Mercury
Molybdenum
Neodymium
Neon
Neptunium
Nickel
Niobium
Nitrogen
Nobelium

Osmium
Oxygen
Palladium
Phosphorus
Platinum
Plutonium
Polonium
Potassium
Praseodymium
Promethium
Protactinium
Radium
Radon
Rhenium
Rhodium
Roentgenium
Rubidium
Ruthenium
Rutherfordium
Samarium
Scandium
Seaborgium
Selenium
Silicon
Silver
Sodium
Strontium
Sulfur
Tantalum
Technetium

Tellurium
Terbium
Thallium
Thorium
Thulium
Tin
Titanium
Tungsten
Ununoctium
Ununpentium
Ununseptium
Ununtrium
Uranium
Vanadium
Xenon
Ytterbium
Yttrium
Zinc
Zirconium


Symbol

Atomic
Number

Atomic
Mass

Md

Hg
Mo
Nd
Ne
Np
Ni
Nb
N
No
Os
O
Pd
P
Pt
Pu
Po
K
Pr
Pm
Pa
Ra
Rn
Re
Rh
Rg
Rb
Ru
Rf
Sm
Sc

Sg
Se
Si
Ag
Na
Sr
S
Ta
Tc
Te
Tb
Tl
Th
Tm
Sn
Ti
W
Uuo
Uup
Uus
Uut
U
V
Xe
Yb
Y
Zn
Zr

101

80
42
60
10
93
28
41
7
102
76
8
46
15
78
94
84
19
59
61
91
88
86
75
45
111
37
44
104
62
21

106
34
14
47
11
38
16
73
43
52
65
81
90
69
50
22
74
118
115
117
113
92
23
54
70
39
30
40

(258)

200.59
95.96
144.242
20.1797
(237)
58.6934
92.90638
14.007
(259)
190.23
15.999
106.42
30.973762
195.084
(244)
(209)
39.0983
140.90765
(145)
231.03588
(226)
(222)
186.207
102.90550
(280)
85.4678
101.07
(265)
150.36
44.955912

(271)
78.96
28.085
107.8682
22.98976928
87.62
32.06
180.94788
(98)
127.60
158.92535
204.38
232.03806
168.93421
118.710
47.867
183.84
(294)
(288)
(294)
(284)
238.02891
50.9415
131.293
173.054
88.90585
65.38
91.224

The values given in parentheses are the atomic mass numbers of the isotopes of the longest known half-life. From M. E. Wieser and T. B.

Coplen, Pure Appl. Chem., 2011, 83(2), 359–96, DOI: 10.1351/PAC-REP-10-09-14.

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Molar Mass

AgBr
AgCl
Ag2CrO4
AgI
AgNO3
AgSCN
Al2O3
Al2(SO4)3
As2O3
B2O3
BaCO3
BaCl2 ? 2H2O
BaCrO4
Ba(IO3)2
Ba(OH)2
BaSO4
Bi2O3
CO2
CaCO3
CaC2O4
CaF2
CaO
CaSO4

Ce(HSO4)4
CeO2
Ce(SO4)2
(NH4)2Ce(NO3)6
(NH4)4Ce(SO4)4 ? 2H2O
Cr2O3
CuO
Cu2O
CuSO4
Fe(NH4)2(SO4)2 ? 6H2O
FeO
Fe2O3
Fe3O4
HBr
HC2H3O2 (acetic acid)
HC7H5O2 (benzoic acid)
(HOCH2)3CNH2 (TRIS)
HCl
HClO4
H2C2O4 ? 2H2O
H5IO6
HNO3
H2O
H2O2
H3PO4
H2S
H2SO3
H2SO4
HgO
Hg2Cl2

HgCl2
KBr
KBrO3
KCl
KClO3
KCN
K2CrO4
K2Cr2O7

187.772
143.32
331.729
234.7727
169.872
165.95
101.960
342.13
197.840
69.62
197.335
244.26
253.319
487.130
171.341
233.38
465.958
44.009
100.086
128.096
78.075

56.077
136.13
528.37
172.114
332.23
548.22
632.53
151.989
79.545
143.091
159.60
392.13
71.844
159.687
231.531
80.912
60.052
122.123
121.135
36.46
100.45
126.064
227.938
63.012
18.015
34.014
97.994
34.08
82.07
98.07

216.59
472.08
271.49
119.002
166.999
74.55
122.55
65.116
194.189
294.182

nds

Molar Masses of Some Compou
Compound

Compound

Molar Mass

K3Fe(CN)6
K4Fe(CN)6
KHC8H4O4 (phthalate)
KH(IO3)2
K2HPO4
KH2PO4
KHSO4
KI
KIO3
KIO4

KMnO4
KNO3
KOH
KSCN
K2SO4
La(IO3)3
Mg(C9H6NO)2
  (8-hydroxyquinolate)
MgCO3
MgNH4PO4
MgO
Mg2P2O7
MgSO4
MnO2
Mn2O3
Mn3O4
Na2B4O7 ? 10H2O
NaBr
NaC2H3O2
Na2C2O4
NaCl
NaCN
Na2CO3
NaHCO3
Na2H2EDTA ? 2H2O
Na2O2
NaOH
NaSCN
Na2SO4
Na2S2O3 ? 5H2O

NH4Cl
(NH4)2C2O4 ? H2O
NH4NO3
(NH4)2SO4
(NH4)2S2O8
NH4VO3
Ni(C4H7O2N2)2
  (dimethylglyoximate)
PbCrO4
PbO
PbO2
PbSO4
P2O5
Sb2S3
SiO2
SnCl2
SnO2
SO2
SO3
Zn2P2O7

329.248
368.346
204.222
389.909
174.174
136.084
136.16
166.0028
214.000

229.999
158.032
101.102
56.105
97.18
174.25
663.610
312.611

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84.313
137.314
40.304
222.551
120.36
86.936
157.873
228.810
381.36
102.894
82.034
133.998
58.44
49.008
105.988
84.006
372.238
77.978
39.997

81.07
142.04
248.17
53.49
142.111
80.043
132.13
228.19
116.978
288.917
323.2
223.2
239.2
303.3
141.943
339.70
60.083
189.61
150.71
64.06
80.06
304.70


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Charles D. Winters

H2O 1 I32(aq) 1 H3AsO3(aq) S
(a)

d 3I2(aq) 1 H3AsO4(aq) 1 H1(aq)
(b)

Charles D. Winters

Color Plate 1 Chemical Equilibrium 1: Reaction between iodine and
arsenic(III) at pH 1. (a) One mmol I3− added to one mmol H3AsO3.
(b) Three mmol I− added to one mmol H3AsO4. Both combinations of
solutions produce the same final equilibrium state (see Section 9B-1, page 202).

H2O 1 I32(aq) 1 H3AsO3(aq) S
(a)

d 3I2(aq) 1 H3AsO4(aq) 1 H1(aq)
(b)

Charles D. Winters

Color Plate 2 Chemical Equilibrium 2: The same reaction as in color
plate 1 carried out at pH 7, producing a different equilibrium state than that
in Color Plate 1, and although similar to the situation in Color Plate 1, the
same state is produced from either the forward (a) or the reverse (b) direction
(see Section 9B-1, page 202).

I32(aq) 1 2Fe(CN)64−(aq) S
(a)

d 3I2(aq) 1 2Fe(CN)63− (aq)
(b)

Color Plate 3 Chemical Equilibrium 3: Reaction between iodine and
ferrocyanide. (a) One mmol I3− added to two mmol Fe(CN)642. (b) Three
mmol I− added to two mmol Fe(CN)632. Both combinations of solutions
produce the same final equilibrium state. (see Section 9B-1, page 202).

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Charles D. Winters

Charles D. Winters

Charles D. Winters

Charles D. Winters

Charles D. Winters

Color Plate 5 Crystallization of sodium acetate from
a supersaturated solution (see Section 12A-2, page 280).
A tiny seed crystal is dropped into the center of a petri dish
containing a supersaturated solution of the compound.
The time sequence of photos taken about once per second
shows the growth of the beautiful crystals of sodium acetate.

Charles D. Winters

Color Plate 4 The common-ion effect.
The test tube on the left contains a saturated
solution of silver acetate, AgOAc. The following
equilibrium is established in the test tube:
AgOAc(s) 8 Ag+(aq) + OAc−(aq)

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When AgNO3 is added to the test tube, the
equilibrium shifts to the left to form more
AgOAc, as shown in the test tube on the right
(see Section 9B-5, page 209).


Charles D. Winters

Color Plate 6 The Tyndall effect. The photo shows
two cuvettes: the one on the left contains only water while
the one on the right contains a solution of starch. As red
and green laser beams pass through the water in the left

cuvette, they are invisible. Colloidal particles in the starch
solution in the right cuvette scatter the light from the two
lasers, so the beams become visible (see Section 12A-2,
margin note, page 280).

Charles D. Winters

Color Plate 7 When dimethylglyoxime
is added to a slightly basic solution of
Ni21(aq), shown on the left, a bright red
precipitate of Ni(C4H7N2O2)2 is formed
as seen in the beaker on the right
(see Section 12C-3, page 294).

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1 2 3 4 5 6 7 8 9 10 11 12
pH
Methyl violet (0.0–1.6)

Chlorophenol red (4.8–6.7)

1 2 3 4 5 6 7 8 9 10 11 12
pH

1 2 3 4 5 6 7 8 9 10 11 12
pH
m-Cresol purple (7.4–9.0)

Bromophenol blue (3.0–4.6)

1 2 3 4 5 6 7 8 9 10 11 12
pH

1 2 3 4 5 6 7 8 9 10 11 12
pH

Methyl orange (3.2–4.4)

Thymol blue (8.0–9.2)

1 2 3 4 5 6 7 8 9 10 11 12
pH

1 2 3 4 5 6 7 8 9 10 11 12
pH

Bromocresol green (3.8–5.4)

Phenolphthalein (8.0–10.0)

1 2 3 4 5 6 7 8 9 10 11 12
pH
Alizarin red (4.6–6.0)

Charles D. Winters

1 2 3 4 5 6 7 8 9 10 11 12
pH

1 2 3 4 5 6 7 8 9 10 11 12
pH
o-Cresolphthalein (8.2–9.8)

1 2 3 4 5 6 7 8 9 10 11 12
pH
Bromothymol (6.0–7.0)

1 2 3 4 5 6 7 8 9 10 11 12
pH
Thymolphthalein (8.8–10.5)

Color Plate 8 Acid/base indicators and their transition pH ranges (see Section 14A-2, page 323).

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Charles D. Winters

Charles D. Winters

Charles D. Winters

Charles D. Winters

Color Plate 11 A modern version of the Daniell Cell
(see Feature 18-2, page 450).

Color Plate 12 Reaction between Iron(III) and

iodide. The species in each beaker are indicated by
the colors of the solutions. Iron (III) is pale yellow,
iodide is colorless, and triiodide is intense red-­
orange (see margin note, Section 18C-6, page 464).

Color Plate 13 The time dependence of the reaction between permanganate and oxalate (see Section 20C-1, page 515).

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Charles D. Winters

Charles D. Winters

2Fe31 1 3I2     8    2Fe21 1 I32

Charles D. Winters

Color Plate 10 Reduction of
silver(I) by direct reaction with
copper, forming the “silver tree”
(see Section 18A-2, page 445).

Color Plate 9 End point in an acid/base titration with phenolphthalein as
indicator. The end point is achieved when the barely perceptible pink color of
phenolphthalein persists. The flask on the left shows the titration less than half a
drop prior to the end point; the middle flask shows the end point. The flask on
the right shows what happens when a slight excess of base is added to the titration mixture. The solution turns a deep pink color, and the end point has been
exceeded (see Section 13A-1, page 304).

© H&H Productions

(b)

Simon Tulloch

Simon Tulloch

(a)

(c)

Charles D. Winters

Color Plate 14 (a) Typical linear CCD arrays for spectrophotometers. The array on the right has 4096 pixels, and the
array on the left has 2048 pixels. In both arrays, each pixel has the dimensions of 14 mm 3 14 mm. These devices have a
spectral range of 200-1000 nm, a dynamic range of 2500:1 (see Section 8E-2), and are available with low-cost glass or
UV-enhanced fused silica windows. In addition to the sizes shown, the arrays are available in lengths of 512 and 1024 pixels.
(b) Photomicrograph of a section of a two-dimensional CCD array that is used for imaging and spectroscopy. Light falling
on the millions of pixels in the upper left of the photo creates charge that is transferred to the vertical channels at the
bottom of the photo and shifted from left to right along the string of channels until it reaches the output amplifier section
shown in (c). The amplifier provides a voltage proportional to the charge accumulated on each pixel, which is in turn
proportional to the intensity of light falling on the pixel (see Section 25A-4, page 705, for a discussion of charge-transfer
devices).
Color Plate 15 Series of standards (left) and two
unknowns (right) for the spectrophotometric determination of Fe(II) using 1,10-phenanthroline as reagent
(see Section 26A-3 and Problem 26-26, page 757).
The color is due to the complex Fe(phen)32+.
The absorbance of the standards is measured, and a
working curve is analyzed using linear least-squares

(see Section 8C-2, page 172). The equation for the
line is then used to determine the concentrations of the
unknown solutions from their measured absorbances.

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Visible Spectrum
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Barium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Calcium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Chromium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Europium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Indium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Iron
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Lithium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Sodium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Strontium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Thallium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

Vanadium
380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

380 400 420 440 460 480 500 520 540 560 580 600 620 640 660 680 700 720

l, nm

Color Plate 16 Spectrum of white light and emission spectra of selected elements
(see Chapter 28).

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Jim Holler

Ytterbium


400

410

420

430

440

450

460

460

470

480

490

500

510

520

520

530

540

550

560

570

580

580

590

600

610

620

630

640

640

650

660

670

680

690

700

l, nm
(a)

H
He

l
(a)
Color Plate 17 The solar spectrum. (a) Expanded color version of the solar spectrum
shown in black and white in Feature 24-1 (see Figure 24F-1, page 657). The huge number
of dark absorption lines are produced by all of the elements in the sun. See if you can
spot some prominent lines like the famous sodium doublet. (b) Compact version of the
solar spectrum in (a) compared to the emission spectra of hydrogen, helium, and iron.
It is relatively easy to spot lines in the emission spectra of hydrogen and iron that
correspond to absorption lines in the solar spectrum, but the lines of helium are quite
obscure. In spite of this problem, helium was discovered when these lines were observed
in the solar spectrum (see Section 28D). (Images created by Dr. Donald Mickey,
University of Hawaii Institute for Astronomy from National Solar Observatory spectral
data/NSO/Kitt Peak FTS data by NSF/NOAO.)

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(Dr. Donald Mickey)

Fe


Charles D. Winters

Color Plate 18 (a) Demonstration
of atomic absorption by mercury vapor.
(b) White light from the source on the
right passes through the mercury vapor
above the flask and no shadow appears
on the fluorescent screen on the left.
Light from the mercury lamp on the
left containing the characteristic UV
lines of the element is absorbed by the
vapor in and above the flask, which casts
a shadow on the screen on the right of
the plume of mercury vapor (see Section
28D-4, page 797).

(a)

Fluorescent screen

Shadow

Mercury vapor

Mercury vapor lamp

White light source

Jim Holler

Liquid
mercury

(b)

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Charles D. Winters

Charles D. Winters



(c)

(b)

Charles D. Winters

(d)

(e)

Color Plate 19 Weighing by
difference the old-fashioned way.

(a) Zero the balance. (b) Place a
weighing bottle containing the
solute on the balance pan. (c) Read
the mass (33.2015 g). (d) Transfer
the desired amount of solute to a flask.
(e) Replace the weighing bottle on the
pan and read the mass (33.0832 g).
Finally, calculate the mass of the
solute transferred to the flask:
33.2015 g 2 33.0832 g 5 0.1131 g
(see Section 2E-4, page 27).
(Electronic balance provided by
Mettler-Toledo, Inc.)





Charles D. Winters

(a)

Charles D. Winters



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(c)

(b)

Charles D. Winters



Charles D. Winters

Charles D. Winters

(a)

Charles D. Winters



(d)

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Color Plate 20 Weighing by difference the modern way. Place a weighing
bottle containing the solute on the
balance pan and (a) depress the tare
or zero button. The balance should
then read 0.0000 g, as shown in (b).
(c) Transfer the desired amount of
solute to a flask. Replace the weighing
bottle on the pan, and (d) the balance
reads the decrease in mass directly as

20.1070 g (see Section 2E-4, page 27).
Many modern balances have built-in
computers with programs to perform a
variety of weighing tasks. For example,
it is possible to dispense many
consecutive quantities of a substance
and automatically read out the loss in
mass following each dispensing.
Many balances also have computer
intterfaces so that reading may be
logged directly to programs running
on the computer. (Electronic balance
provided by Mettler-Toledo, Inc.)


1019

Gamma
rays

10212
(1 pm)

1018

1017

X rays

10211

(10 pm)

10210
(100 pm)

1029
(1 nm)

1016
Far
ultraviolet

1028
(10 nm)

1015
Near
ultraviolet

1027
(100 nm)

1014
Visible

1020

1026
(1 mm)

1013

Near
infrared

1012

Far
infrared

1025
(10 mm)

1024
(100 mm)

1011

1010

Microwaves

1023
(1 mm)

1022
(10 mm)

Frequency (s21)

TV FM AM
Radio waves

Radar

Wavelength (m)
1021
(100 mm)

Visible spectrum

350

400

450

500

550

600

650

700

750

Color Plate 21 Electromagnetic spectrum. The spectrum extends from high-energy (frequency) gamma rays to low-energy (frequency) radio waves (see

Section 24B-1, page 654). Note that the visible region is only a tiny fraction of the spectrum. The visible region, broken out in the lower portion, e­ xtends
from the violet (≈380 nm) to the red region (≈800 nm). (Courtesy of Ebbing and Gammon, General Chemistry, 10th ed.)

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800
nm


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Fundamentals of
Analytical
Chemistry
Douglas A. Skoog
Stanford University

Donald M. West
San Jose State University

F. James Holler
University of Kentucky

Stanley R. Crouch
Michigan State University

Australia • Brazil • Japan • Korea • Mexico • Singapore • Spain • United Kingdom • United States

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ninth Edition


Fundamentals of Analytical Chemistry,
Ninth Edition
Douglas A. Skoog, Donald M. West, F. James
Holler, Stanley R. Crouch
Publisher: Mary Finch
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Developmental Editor: Sandra Kiselica

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Contents in Brief
Chapter 1

The Nature of Analytical Chemistry  1

Part I Tools of Analytical Chemistry 14
Chapter 2
Chemicals, Apparatus, and Unit Operations of
Analytical Chemistry  15
Chapter 3
Using Spreadsheets in Analytical Chemistry  48
Chapter 4
Calculations Used in Analytical Chemistry  62
Chapter 5
Errors in Chemical Analyses  82
Chapter 6
Random Errors in Chemical Analysis  93
Chapter 7
Statistical Data Treatment and Evaluation  123
Chapter 8
Sampling, Standardization, and Calibration  153
Part II  Chemical Equilibria 196
Chapter 9
Aqueous Solutions and Chemical Equilibria  197
Chapter 10 Effect of Electrolytes on Chemical Equilibria  235
Chapter 11 Solving Equilibrium Problems for
Complex Systems  249
Part III Classical Methods of Analysis 279
Chapter 12 Gravimetric Methods of Analysis 280
Chapter 13 Titrations in Analytical Chemistry 302
Chapter 14 Principles of Neutralization Titrations 322
Chapter 15 Complex Acid/Base Systems 348

Chapter 16 Applications of Neutralization Titrations 381
Chapter 17 Complexation and Precipitation Reactions
and Titrations 400
Part IV Electrochemical Methods 441
Chapter 18 Introduction to Electrochemistry 442
Chapter 19 Applications of Standard Electrode Potentials 473
Chapter 20 Applications of Oxidation/Reduction Titrations 509
Chapter 21 Potentiometry 535
Chapter 22 Bulk Electrolysis: Electrogravimetry and Coulometry 578
Chapter 23 Voltammetry 610
Part V Spectrochemical Methods 649
Chapter 24 Introduction to Spectrochemical Methods 650
Chapter 25 Instruments for Optical Spectrometry 683
Chapter 26 Molecular Absorption Spectrometry 722
Chapter 27 Molecular Fluorescence Spectroscopy 760
Chapter 28 Atomic Spectroscopy 773
Chapter 29 Mass Spectrometry  802
   iii

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iv  Contents in Brief
Part VI Kinetics and Separations 818
Chapter 30 Kinetic Methods of Analysis  819
Chapter 31 Introduction to Analytical Separations  847
Chapter 32 Gas Chromatography  887
Chapter 33 High-Performance Liquid Chromatography  912
Chapter 34 Miscellaneous Separation Methods  935
Part VII Practical Aspects of Chemical Analysis 959

Part VII chapters are only available as an Adobe Acrobat® PDF file on the web at
www.cengage.com/chemistry/skoog/fac9.
Chapter 35
Chapter 36
Chapter 37
Chapter 38

The Analysis of Real Samples  960
Preparing Samples for Analysis  970
Decomposing and Dissolving the Sample  976
Selected Methods of Analysis  986
Glossary  G-1

Appendix 1
Appendix 2
Appendix 3
Appendix 4
Appendix 5
Appendix 6
Appendix 7
Appendix 8
Appendix 9

The Literature of Analytical Chemistry  A-1
Solubility Product Constants at 25°C  A-6
Acid Dissociation Constants at 25°C  A-8
Formation Constants at 25°C  A-10
Standard and Formal Electrode Potentials  A-12
Use of Exponential Numbers and Logarithms  A-15
Volumetric Calculations Using Normality and Equivalent

Weight  A-19
Compounds Recommended for the Preparation of Standard
Solutions of Some Common Elements  A-27
Derivation of Error Propagation Equations  A-29
Answers to Selected Questions and Problems  A-34
Index  I-1

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