Appendix E
Chemistry Data Tables
Table E.4 Conversion Factors
Quantity
Relationships between units
Table E.1 Useful Math Relationships
D=
m
V
P=
F
A
length
π = 3.1416
1 m = 10−3 km
= 103 mm
= 102 cm
1 pm = 10−12 m
Volume of sphere V =
4 3
πr
3
mass
1 u = 1.66 × 10−27 kg
Table E.2 Fundamental Physical Constants (to six
significant digits)
acceleration due to gravity (g )
9.806 65 m/s2
Avogadro constant (Na)
6.022 14 × 1023/mol
charge on one mole of
electrons (Faraday constant)
96 485.3 C/mol
mass of electron (ms)
9.109 38 × 10−31 kg
mass of neutron (mn)
1.674 93 × 10−27 kg
mass of proton (mp)
1.672 62 × 10−27 kg
molar gas constant (R )
8.314 47 J/mol·K
molar volume of gas at STP
22.414 0 L/mol
speed of light in vacuo (c )
2.997 92 × 10 m/s
unified atomic mass (u )
1.660 54 × 10−27 kg
temperature
1012
giga (G)
109
mega (M)
106
kilo (k)
103
deci (d)
10−1
centi (c)
10−2
milli (m)
10−3
micro (µ)
10−6
nano (n)
10−9
pico (p)
10−12
0 K = −273.15˚C
T (K) = T (˚C) + 273.15
T (˚C) = T (K) − 273.15
mp of H2O = 273.15 K (0˚C)
bp of H2O = 373.15 K (100˚C)
volume
1 L = 1 dm3
= 10−3 m3
8
= 103 mL
1 mL = 1 cm3
Table E.3 Common SI Prefixes
tera (T)
1 kg = 103 g
= 10−3 t
Volume of cylinder = πr h
2
pressure
101 325 Pa = 101.325 kPa
= 760 mm Hg
= 760 torr
= 1 atm
density
1 kg/m3 = 103 g/m3
= 10−3 g/mL
= 1 g/L
energy
1 J = 6.24 × 1018 eV
Appendix E • MHR
595
Table E.5 Alphabetical Listing of Common Polyatomic Ions
Most common ion
acetate
Common related ions
+
NH4
arsenate
AsO43−
if the ion is the most
common oxoanion
-ate
chlorate, ClO3−
-ite
chlorite, ClO2−
tetraborate
B4O72−
if the ion has one O
atom less than the most
common oxoanion
HCO3−
hypochlorite,
ClO−
bicarbonate
(hydrogen
carbonate)
if the ion has two O
hypo-___-ite
atoms less than the most
common oxoanion
per-___-ate
perchlorate
chlorite
hypochlorite
ClO4−
ClO2−
ClO−
if the ion has 1 O
atom more than the
most common oxoanion
perchlorate,
ClO4−
bi-
CrO42−
dichromate
Cr2O72−
if the ion has 1 H atom
added to the most
common oxoanion
bicarbonate,
HCO3−
−
cyanate
thiocyanate
OCN−
SCN−
if the ion has 1 O atom
less and 1 S atom more
than the most common
oxoanion
thio-
thiosulphate,
S2O32−
if the ion has the higher
possible charge
-ic
titanic, Ti4+
if the ion has the lower
possible charge
-ous
cuprous, Cu+
Note: According to the
Stock system, metallic
ions are named using
Roman numerals.
The Roman
numeral shows
the charge on
the metal ion
titanium(IV) Ti4+
copper(I), Cu+
manganese(VII),
Mn7 +
borate
BO33−
−
3−
bromate
BrO3
carbonate
CO32−
ClO3−
cyanide
CN
glutamate
C5H8NO4−
hydroxide
OH−
peroxide
O22−
iodate
IO3−
iodide
I−
nitrate
NO3−
nitrite
NO2−
oxalate
OOCCOO2−
Metallic Ions
−
permanganate
MnO4
phosphate
PO43−
silicate
SiO32−
phosphite
PO33−
tripolyphosphate P3O105−
orthosilicate
SiO44−
bisulfate
(hydrogen
sulfate)
sulfite
bisulfite
(hydrogen
sulfite)
thiosulfate
HSO4−
bisulfide
(hydrogen
sulfide)
HS−
−
stearate
C17H35COO
sulfate
SO42−
sulfide
Example
AsO33−
C6H5COO
chromate
Prefix or suffix
arsenite
benzoate
chlorate
Type of ion
Polyatomic Ions
CH3COO−
ammonium
Table E.6 Summary of Naming Rules for Ions
S2−
596 MHR • Appendix E
SO32−
HSO3−
2−
S 2 O3
Table E.7 Summary of Naming Rules for Acids
Modern name
Classical acid name
Example
aqueous
hydrogen ___ide
hydro___ic acid
HCl, aqueous
hydrogen chloride
or hydrochloric acid
aqueous
hydrogen ___ate
___ic acid
H2CO3, aqueous
hydrogen carbonate
or carbonic acid
aqueous
hydrogen ___ite
___ous acid
HNO2, aqueous
hydrogen nitrite
or nitrous acid
Table E.8 Standard Molar Enthalpies of Formation
Substance
∆H ˚f
(kJ/mol)
∆H ˚f
Substance (kJ/mol)
Acid
∆H ˚f
Substance (kJ/mol)
Formula
Ka
Conjugate base
hypochlorous
acid
HClO
ClO−
4.0 × 10−8
IO3−
1.7 × 10−1
Al2O3(s)
−1675.7 HBr(g)
−36.3 NH3(g)
−45.9
iodic acid
HIO3
CaCO3(s)
−1207.6 HCl(g)
−92.3 N2H4()
+50.6
lactic acid
CH3CHOHCO2H CH3CHOHCO2− 1.4 × 10−4
CaCl2(s)
−795.4 HF(g)
−273.3 NH4Cl(s)
−314.4
methanoic acid HCOOH
Ca(OH)2(s)
−985.2 HCN(g)
+135.1 NH4NO3(s)
−365.6
nitric acid
CCl4()
−128.2 H2O()
−285.8 NO(g)
+91.3
CCl4(g)
−95.7 H2O(g)
−241.8 NO2(g)
+33.2
−134.1 H2O2()
−187.8 N2O(g)
+81.6
−174.1 N2O4(g)
+11.1
CHCl3()
CH4(g)
−74.6 HNO3()
C2H2(g)
+227.4 H3PO4(s)
C2H4(g)
+52.4 H2S(g)
C2H6(g)
C3H8(g)
−84.0 H2SO4()
−103.8 FeO(s)
−1284.4 PH3(g)
+5.4
−20.6 PCl3(g)
−287.0
−814.0 P4O6(s)
−2144.3
−272.0 P4O10(s)
−2984.0
+49.1 Fe2O3(s)
−824.2 KBr(s)
−393.8
CH3OH()
−239.2 Fe3O4(s)
−1118.4 KCl(s)
−436.5
C2H5OH()
−277.6 FeCl2(s)
−341.8 KClO3(s)
−397.7
CH3COOH()
−484.3 FeCl3(s)
−399.5 KOH(s)
−424.6
CO(g)
−110.5 FeS2(s)
−178.2 Ag2CO3(s)
−505.8
CO2(g)
−393.5 PbCl2(s)
−359.4 AgCl(s)
−127.0
COCl2(g)
−219.1 MgCl2(s)
−641.3 AgNO3(s)
−124.4
C6H6()
+89.0 MgO(s)
CS2()
CS2(g)
+116.7 Mg(OH)2(s)
CrCl3(s)
−601.6 Ag2S(s)
−32.6
HCOO−
1.8 × 10−4
HNO3
NO3−
2.4 × 101
nitrous acid
HNO2
NO2
−
phenol
C6H5OH
C6H5O−
5.6 × 10−4
1.0 × 10−10
Table E.10 Ionization Constants for Polyprotic Acids
Acid
Formula
Ka
Conjugate base
boric acid
H3BO3
(aqueous
H2BO3−
hydrogen borate)
H2BO3−
HBO32−
5.4 × 10−10
<1.0 × 10−14
carbonic acid
HCO3−
CO32−
4.5 × 10−7
4.7 × 10−11
H2 C 6H5 O7−
HC6H5O72−
C6H5O73−
7.4 × 10−4
1.7 × 10−5
4.0 × 10−7
H2CO3
HCO3−
H3 C 6H5 O7
citric acid
H2 C 6H5 O7−
(aqueous
hydrogen citrate) HC6H5O72−
oxalic acid
HOOCCOOH HOOCCOO−
HOOCCOO− OOCCOO2−
phosphoric acid
(aqueous
hydrogen
phosphate)
H3PO4
H2PO4−
HPO42−
H2PO4−
HPO42−
PO43−
6.9 × 10−3
6.2 × 10−8
4.8 × 10−13
H2 S
HS−
HS−
S2−
8.9 × 10−8
1.0 × 10−19
5.6 × 10−2
1.5 × 10−4
−924.5 SF6(g)
−1220.5
−556.5 HgS(s)
−58.2 SO2(g)
−296.8
hydrosulfuric
acid
Cu(NO3)2(s)
−302.9 NaCl(s)
−411.2 SO3(g)
−395.7
sulfuric acid
CuO(s)
−157.3 NaOH(s)
−425.6 SnCl2(s)
−325.1
H2SO4
HSO4−
HSO4−
SO42−
1.0 × 103
1.0 × 10−2
CuCl(s)
−137.2 Na2CO3(s)
−1130.7 SnCl4()
−511.3
sulfurous acid
H2SO3
HSO3−
HSO3−
SO32−
1.4 × 10−2
6.3 × 10−8
CuCl2(s)
−220.1
tartaric acid
H2 C 4H4 O6
HC4H4O6−
HC4H4O6−
C4H4O62−
9.3 × 10−4
4.3 × 10−5
Note: The enthalpy of formation of an element in its
standard state is defined as zero.
Table E.11 Ionization Constants for Nitrogen Bases
Table E.9 Ionization Constants for Acids
Acid
Formula
Conjugate base
Ka
acetic acid
CH3COOH
CH3COO−
1.8 × 10−5
benzoic acid
C6H5COOH
C6H5COO−
6.3 × 10−5
−
1.1 × 10−2
chlorous acid
HClO2
ClO2
cyanic acid
HOCN
OCN−
−
Base
Formula
Conjugate
acid
(CH3)2NH
(CH3)2NH2+
5.4 × 10−4
3.5 × 10−4
dimethylamine
(N-methylmethanamine)
1.8 × 10−4
ethanamine
C2H5NH2
C2H5NH3+
4.5 × 10−4
1.0 × 109
methanamine
CH3NH2
CH3NH3+
4.6 × 10−4
formic acid
HCHO2
CHO2
hydrobromic
acid
HBr
Br−
1.3 × 106
trimethylamine
(N-N-dimethylmethanamine)
(CH3)3NH
HCl
Cl−
(CH3)3N
hydrochloric
acid
hydrocyanic
acid
HCN
CN−
6.2 × 10−10
ammonia
NH3
NH4+
6.3 × 10−4
N2 H4
N2 H5+
HF
F−
hydrazine
hydrofluoric
acid
OH−
BrO−
hydrogen oxide H2O
hypobromous
acid
HOBr
Kb
1,2-diaminoethane NH2CH2CH2NH2 NH2CH2
(ethylenediamine)
CH2NH3+ 8.4 × 10−5
+
6.4 × 10−5
1.8 × 10−5
1.3 × 10−6
+
8.8 × 10−9
hydroxylamine
NH2OH
NH3OH
1.0 × 10−14
pyridine
C5H5N
C5H5NH+
2.8 × 10−9
aniline
C6H5NH2
C6H5NH3
urea
NH2CONH2
NH2CONH3+ 1.3 × 10−14
1.7 × 10−9
+
7.5 × 10−10
continued…
Appendix E • MHR
597
Table E.12 Solubility Product Constants in Water at 25˚C
−5
5.38 × 10
1.10 × 10−4
AgBrO3
TlBrO3
Bromides
5.35 × 10−13
6.27 × 10−9
6.60 × 10−6
AgBr
CuBr
PbBr2
Carbonates
8.46 × 10−12
2.58 × 10−9
3.36 × 10−9
6.82 × 10−6
7.40 × 10−14
Ag2CO3
BaCO3
CaCO3
MgCO3
PbCO3
6.92 × 10
7.2 × 10−15
5.02 × 10−6
5.92 × 10−15
9.38 × 10−27
4.87 × 10−17
2.79 × 10−39
1.43 × 10−20
5.61 × 10−12
5.48 × 10−16
5.45 × 10−27
3 × 10−17
1.77 × 10−10
1.72 × 10−9
Iodides
−12
1.12 × 10
1.12 × 10−10
2.3 × 10−13
Ag2CrO4
BaCrO4
PbCrO4
−12
1.27 × 10
9.8 × 10−9
8.52 × 10−17
CuI
PbI2
AgI
Cyanides
Phosphates
5.97 × 10−17
3.47 × 10−20
AgCN
CuCN
Fluorides
1.84 × 10−7
6.44 × 10−3
3.45 × 10−11
2.36 × 10−6
BaF2
CdF2
CaF2
FeF2
9.84 × 10−21
2.07 × 10−33
2.05 × 10−35
1.40 × 10−37
4.74 × 10−32
AlPO4
Ca3(PO4)2
Co3(PO4)2
Cu3(PO4)2
Ni3(PO4)2
1.08 × 10−10
4.93 × 10−5
6.5 × 10−7
1.08 × 10−13
4.39 × 10−23
−
F2(g) + 2e− 2F (aq)
2.866
Co3+(aq) + e− Co2+(aq)
1.92
H2O2(aq) + 2H+(aq) + 2e− 2H2O()
1.776
Ce4+(aq) +
−
e Ce
3+
1.72
(aq)
PbO2(s) + 4H+ (aq) + SO42−(aq) + 2e− PbSO4(s) + H2O()
−
MnO4
(aq) +
+
8H
(aq) +
−
(aq) +
2+
5e Mn
4H2O()
Au3+(aq) + 3e− Au(s)
+
PbO2(s) + 4H
(aq) +
2e Pb
(aq) +
2+
2H2O()
Cl2(g) + 2e− 2Cl− (aq)
(aq) +
2−
Cr2O7
+
−
6e 2Cr
(aq) +
3+
7H2O()
O2(g) + 4H+(aq) + 4e− 2H2O()
+
MnO2(s) + 4H
(aq) +
−
2e Mn
(aq) +
2H2O()
−
Br2() + 2e 2Br
1.224
1.085
1.002
−
0.957
2+
2Hg2+(aq) + 2e− Hg2 (aq)
0.920
NO3
(aq) +
+
1.232
1.066
(aq)
−
AuCl4−(aq) + 3e− Au(s) + 4Cl (aq)
−
1.455
1.229
2+
IO3−(aq) + 6H+ (aq) + 6e− I−(aq) + 3H2O()
−
1.507
1.358
(aq) +
14H
1.691
1.498
−
4H
(aq) +
3e NO(g) + 2H2O()
continued…
598 MHR • Appendix E
(aq) +
0.771
2e H2O2(aq)
−
I2(s) + 2e− 2I (aq)
+
(aq) +
Cu
e Cu(s)
0.521
−
(aq) +
2+
Cu
2e Cu(s)
(aq) +
2−
SO4
0.222
−
2e H2SO3(aq) + H2O()
+
Cu2+(aq) + e− Cu (aq)
+
0.172
0.153
−
(aq) +
0.401
0.342
−
AgCl(s) + e− Ag(s) + Cl (aq)
(aq) +
0.695
0.536
−
−
O2(g) + 2H2O() + 4e− 4OH (aq)
2e H2(g)
0.000
Fe3+(aq) + 3e− Fe(s)
−0.037
Pb2+(aq) + 2e− Pb(s)
−0.126
Sn2+(aq) + 2e− Sn(s)
−0.138
2H
−
(aq) +
2+
Ni
−0.257
2e Ni(s)
Cd2+(aq) + 2e− Cd(s)
−
(aq) +
3+
Cr
−0.403
−0.407
2+
e Cr
(aq)
Fe2+(aq) + 2e− Fe(s)
3e Cr(s)
(aq) +
Cr
−0.447
−
3+
−0.744
Zn2+(aq) + 2e− Zn(s)
−0.762
−
2H2O() + 2e H2(g) + 2OH
Al3+(aq) + 3e− Al(s)
(aq) +
2+
Mg
+
(aq) +
Na
−
2e Mg(s)
−
e Na(s)
Ca2+(aq) + 2e− Ca(s)
(aq) +
Ba
E ˚(V)
Reduction half reaction
O2(g) + 2H
2+
Table E.13 Standard Reduction Potentials
0.797
−
La3+(aq) + 3e− La(s)
Thiocyanates
CuSCN
Pd(SCN)2
2e 2Hg()
2+
Fe3+(aq) + e− Fe (aq)
+
E ˚(V)
0.800
−
−
Sulfates
BaSO4
CaSO4
Hg2SO4
Hg2
4H
4.01 × 10−9
6.47 × 10−6
1.14 × 10−7
1.12 × 10−10
Chromates
(aq) +
2+
+
Iodates
Ba(IO3)2
Ca(IO3)2
Sr(IO3)2
Y(IO3)3
Chlorides
AgCl
CuCl
−22
Be(OH)2
Cd(OH)2
Ca(OH)2
Co(OH)2
Eu(OH)3
Fe(OH)2
Fe(OH)3
Pb(OH)2
Mg(OH)2
Ni(OH)2
Sn(OH)2
Zn(OH)2
Reduction half reaction
Ag+(aq) + e− Ag(s)
Hydroxides
Bromates
−
2e Ba(s)
K+(aq) + e− K(s)
+
Li
(aq) +
−
e Li(s)
(aq)
−0.828
−1.662
−2.372
−2.379
−2.711
−2.868
−2.912
−2.931
−3.040
Table E.14 Specific Heat Capacities of Various
Substances
Energy
Energy
Energy
Bond (kJ/mol) Bond (kJ/mol) Bond (kJ/mol) Bond
Oxygen
Specific heat capacity
(J/g ·˚C at 25˚C)
Substance
Element
Silicon
Halogens
Energy
(kJ/mol)
Multiple bonds
O—O
204
Si—Si
226
F—Cl
256
C
C
607
O—F
222
Si—P
364
F—Br
280
C
N
615
aluminum
0.900
O—Si
368
Si—S
226
F—I
272
C
O
745
carbon (graphite)
0.711
O—P
351
Si—F
553
Cl—Br
217
N
N
418
copper
0.385
O—S
265
Si—Cl
381
Cl—I
211
N
O
631
gold
0.129
O—Cl
269
Si—Br
368
Br—I
179
O
O
498
14.267
O—Br
235
Si—I
293
F—F
159
C
C
839
O—I
249
Si O
640
hydrogen
iron
0.444
Compound
ammonia (liquid)
4.70
ethanol
2.46
water (solid)
2.01
water (liquid)
4.184
water (gas)
2.01
243
C
N
891
193
C
O
1077
I—I
151
N
N
945
Note: The values in this table represent average values
for the dissociation of bonds between the pairs of atoms
listed. The true values may vary for different molecules.
Table E.16 Average Bond Lengths
Other material
air
1.02
concrete
0.88
glass
0.84
granite
0.79
wood
1.76
Bond
Energy
Energy
Energy
Bond (kJ/mol) Bond (kJ/mol) Bond (kJ/mol) Bond
Carbon
Nitrogen
Length
(pm)
Hydrogen
Table E.15 Average Bond Energies
Hydrogen
Cl—Cl
Br—Br
Energy
(kJ/mol)
Phosphorus
and sulfur
Bond
Length
(pm)
Carbon
Bond
Length
(pm)
Bond
Length
(pm)
Phosphorus
and sulfur
Nitrogen
H—H
74
C—C
154
N—N
146
P—P
221
H—C
109
C—N
147
N—O
144
P—S
210
H—N
101
C—O
143
N—F
139
P—F
156
H—O
96
C—F
133
N—Si
172
P—Cl
204
H—F
92
C—Si
186
N—P
177
P—Br
222
H—Si
148
C—P
187
N—S
168
P—I
243
H—P
142
C—S
181
N—Cl
191
S—S
204
H—S
134
C—Cl
177
N—Br
214
S—F
158
H—Cl
127
C—Br
194
N—I
222
S—Cl
201
H—Br
141
C—I
213
S—Br
225
H—I
161
S—I
234
H—Mg
173
H—H
436
C—C
347
N—N
160
P—P
210
H—C
338
C—N
305
N—O
201
P—S
444
H—N
339
C—O
358
N—F
272
P—F
490
O—O
148
Si—Si
234
F—Cl
166
C
C
134
H—O
460
C—F
552
N—Si
330
P—Cl
331
O—F
142
Si—P
227
F—Br
178
C
N
127
H—F
570
C—Si
305
N—P
209
P—Br
272
O—Si
161
Si—S
210
F—I
187
C
O
123
H—Si
299
C—P
264
N—S
464
P—I
184
O—P
160
Si—F
156
Cl—Br
214
N
N
122
H—P
297
C—S
259
N—Cl
200
S—S
266
O—S
151
Si—Cl
204
Cl—I
243
N
O
120
H—S
344
C—Cl
397
N—Br
276
S—F
343
O—Cl
164
Si—Br
216
Br—I
248
O
O
121
H—Cl
432
C—Br
280
N—I
159
S—Cl
277
O—Br
172
Si—I
240
F—F
143
C
C
121
H—Br
366
C—I
209
S—Br
218
O—I
194
Cl—Cl
199
C
N
115
H—I
298
S—I
170
Br—Br
228
C
O
113
H—Mg
126
I—I
266
N
N
110
continued…
Oxygen
Silicon
Halogens
Multiple bonds
Note: The values in this table are average values. The
length of a bond may be slightly different in different
molecules, depending on the intramolecular forces
within the molecules.
Appendix E • MHR
599