chem30 databook 2010

Data Booklet
Updated 2010

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Table of Common Polyatomic Ions

1 1.01 acetate (ethanoate) CH3COO – chromate CrO42 – phosphate PO43 –
1+,1– ammonium NH4+ dichromate Cr2O72 – hydrogen phosphate HPO42 –
benzoate C6H5COO – cyanide CN – dihydrogen phosphate H2PO4–
2.2 borate BO33 – hydroxide silicate SiO32 –
carbide C22 – iodate OH – sulfate SO42 –
H carbonate CO32 – nitrate hydrogen sulfate HSO4–
hydrogen hydrogen carbonate HCO3– nitrite IO3– sulfite SO32 –
perchlorate CIO4– oxalate NO3– hydrogen sulfite HSO3–
3 6.94 4 9.01 chlorate CIO3– hydrogen oxalate NO2– hydrogen sulfide HS –
1+ 2+ chlorite CIO2– permanganate OOCCOO2 –
1.0 1.6 hypochlorite OCl – or CIO – peroxide
persulfide HOOCCOO–
Li Be
MnO4–
lithium beryllium O22 –
S22 –
11 22.99 12 24.31 thiocyanate SCN –
1+ 2+
thiosulfate S2O32 –

0.9 1.3

Na Mg
sodium magnesium

19 39.10 20 40.08 21 44.96 22 47.87 23 50.94 24 52.00 25 54.94 26 55.85 27 58.93
1+ 2+ 3+ 4+, 3+ 5+, 4+ 3+, 2+ 2+, 4+ 3+, 2+ 2+, 3+
0.8 1.0 1.4 1.5 1.6 1.7 1.6 1.8
1.9
K Ca Sc Ti V Cr Mn Fe
Co
potassium calcium scandium titanium vanadium chromium manganese iron cobalt

37 85.47 38 87.62 39 88.91 40 91.22 41 92.91 42 95.94 43 (98) 44 101.07 45 102.91
1+ 2+ 3+ 4+ 5+, 3+ 6+ 7+ 3+ 3+
0.8 1.0 1.2 1.3 1.6 2.2 2.1 2.2 2.3

Rb Sr Y Zr Nb Mo Tc Ru Rh

rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium

55 132.91 56 137.33 57 138.91 72 178.49 73 180.95 74 183.84 75 186.21 76 190.23 77 192.22
1+ 2+ 3+ 4+ 5+ 6+ 7+ 4+ 4+
0.8 0.9 1.1 1.3 1.5 1.7 1.9 2.2 2.2

Cs Ba La Hf Ta W Re Os Ir

cesium barium lanthanum hafnium tantalum tungsten rhenium osmium iridium

87 (223) 88 (226) 89 (227) 104 (261) 105 (262) 106 (266) 107 (264) 108 (277) 109 (268)
1+ 2+ 3+ 4+

0.7 0.9 1.1

Fr Ra Ac Rf Db Sg Bh Hs Mt
francium radium actinium rutherfordium dubnium seaborgium bohrium hassium meitnerium

lanthanide and actinide series begin

References 58 140.12 59 140.91 60 144.24 61 (145) 62 150.36
3+ 3+ 3+ 3+ 3+, 2+
Lide, D.R. 2005. CRC Handbook of Chemistry
and Physics. 86th ed. Boca Raton: CRC Press. 1.1 1.1 1.1 — 1.2

Speight, James G. 2005. Lange’s Handbook of Ce Pr Nd Pm Sm
Chemistry. 16th ed. New York: McGraw-Hill, Inc. cerium praseodymium neodymium promethium samarium

IUPAC commission on atomic weights and 90 232.04 91 231.04 92 238.03 93 (237) 94 (244)
isotopic abundances. 2002. http://www.chem. 4+ 5+, 4+ 6+, 4+ 5+
qmw.ac.uk/iupac/AtWt/index.html. 1.3 4+, 6+

1.3 1.5 1.7 1.3

Th Pa U Np Pu
thorium protactinium uranium neptunium plutonium

10 11 12 13 14 15 16 17 18

Legend for Elements

Metallic solids Gases 2 4.00
—
Non-metallic solids Liquids —

Key *Atomic molar Note: The legend denotes the physical state of the elements He
at exactly 101.325 kPa and 298.15 K.
26 55.85 mass (g/mol) helium
Atomic number 3+, 2+ Most stable 5 10.81 6 12.01 7 14.01 8 16.00 9 19.00
1.8 ion charges — — —— — 10 20.18
Electronegativity 2.0 2.6 4.0 —
Symbol Fe 3.0 3.4 —
Name B C F
iron NO Ne
boron carbon nitrogen oxygen fluorine
neon

( * Based on m126aCss of the 13 26.98 14 28.09 15 30.97 16 32.07 17 35.45 18 39.95
3+ — — — — —
) Indicates 1.6 1.9 2.2 2.6 3.2 —
most stable isotope
Al Si P S Cl Ar

aluminium silicon phosphorus sulfur chlorine argon

28 58.69 29 63.55 30 65.41 31 69.72 32 72.64 33 74.92 34 78.96 35 79.90 36 83.80
2+, 3+ 2+, 1+ 2+ 3+ 4+ ——— —
1.9
1.9 1.7 1.8 2.0 2.2 2.6 3.0 —
Ni
Cu Zn Ga Ge As Se Br Kr
nickel arsenic selenium bromine krypton
copper zinc gallium germanium
52 127.60 53 126.90 54 131.29
46 106.42 47 107.87 48 112.41 49 114.82 50 118.71 51 121.76 — — —
2+, 3+ 1+ 2+ 3+ 4+, 2+ 3+, 5+ 2.1 2.7 2.6
2.2 1.9 2.1
1.7 1.8 2.0 Te I Xe
Pd Ag Sb
Cd In Sn tellurium iodine xenon
palladium silver cadmium indium tin antimony
85 (210) 86
78 195.08 79 196.97 80 200.59 81 204.38 82 207.2* 83 208.98 84 (209) — (222)
4+, 2+ 3+, 1+ 2+, 1+ 1+, 3+ 2+, 4+ 3+, 5+ 2+, 4+ 2.2 —
—
At
2.2 2.4 1.9 1.8 1.8 1.9 2.0 902 Rn

Pt Au Hg Tl Pb Bi Po 254
platinum gold mercury thallium lead bismuth polonium astatine radon

110 (271) 111 (272) * The isotopic mix of naturally occurring lead is more variable than other
elements, preventing precision to greater than tenths of a gram per mole.
——
——

Ds Rg

darmstadtium roentgenium

63 151.96 64 157.25 65 158.93 66 162.50 67 164.93 68 167.26 69 168.93 70 173.04 71 174.97
3+, 2+ 3+ 3+ 3+ 3+ 3+ 3+ 3+, 2+ 3+

— 1.2 — 1.2 1.2 1.2 1.3 — 1.0

Eu Gd Tb Dy Ho Er Tm Yb Lu

europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium

95 (243) 96 (247) 97 (247) 98 (251) 99 (252) 100 (257) 101 (258) 102 (259) 103 (262)
3+, 4+ 3+ 3+, 4+ 3+ 3+ 3+ 2+, 3+ 2+, 3+ 3+
—
———— Es —— ——

Am Cm Bk Cf Fm Md No Lr
americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium

Chemistry Notation

Symbol Term Unit(s)

c specific heat capacity J/(g.°C) or J/(g.K)

E° standard electrical potential V or J/C
Ek kinetic energy kJ
Ep potential energy kJ
∆H enthalpy (heat) kJ
∆fH° standard molar enthalpy of formation
I current kJ/mol
Kc equilibrium constant A or C/s
Ka acid ionization (dissociation) constant
Kb base ionization (dissociation) constant —
M molar mass —
m mass —
n amount of substance g/mol
P pressure g
Q charge mol
T temperature (absolute) kPa
t temperature (Celsius) C
t time K
V volume °C
c amount concentration s
L
mol/L

Symbol Term

∆ delta (change in)
° standard
[ ] amount concentration

2

Miscellaneous

25.00 °C is equivalent to 298.15 K

Specific Heat Capacities at 298.15 K and 100.000 kPa

cair = 1.01 J/(g.°C)
cpolystyrene foam cup = 1.01 J/(g.°C)

ccopper = 0.385 J/(g.°C)
caluminium = 0.897 J/(g.°C)

ciron = 0.449 J/(g.°C)
ctin = 0.227 J/(g.°C)
cwater = 4.19 J/(g.°C)

Water Autoionization Constant (Dissociation Constant)
Kw = 1.0 × 10–14 at 298.15 K (for ion concentrations in mol/L)

Faraday Constant
F = 9.65 × 104 C/mol e–

Quadratic Formula

x = -b ! b2 - 4ac
2a

Selected SI Prefixes

Prefix Exponential Value
tera Symbol
giga T 1012
mega G 109
kilo M 106
milli k 103
micro m 10–3
nano µ 10–6
pico n 10–9
p 10–12

3

Standard Molar Enthalpies of Formation at 298.15 K

Name Formula ∆f H° (kJ/mol)

aluminium oxide Al2O3(s) –1 675.7
ammonia NH3(g) –45.9
ammonium chloride NH4Cl(s) –314.4
ammonium nitrate NH4NO3(s) –365.6
barium carbonate BaCO3(s)
barium chloride BaCl2(s) –1 213.0
barium hydroxide Ba(OH)2(s) –855.0
barium oxide BaO(s) –944.7
barium sulfate BaSO4(s) –548.0
benzene C6H6(l)
butane C4H10(g) –1 473.2
calcium carbonate CaCO3(s) +49.1
calcium chloride CaCl2(s) –125.7
calcium hydroxide Ca(OH)2(s)
calcium oxide CaO(s) –1 207.6
calcium sulfate CaSO4(s) –795.4
carbon dioxide CO2(g) –985.2
carbon monoxide CO(g) –634.9
chromium(III) oxide Cr2O3(s)
copper(I) oxide Cu2O(s) –1 434.5
copper(II) oxide CuO(s) –393.5
copper(II) sulfate CuSO4(s) –110.5
copper(I) sulfide Cu2S(s)
copper(II) sulfide CuS(s) –1 139.7
dinitrogen tetroxide N2O4(g) –168.6
ethane C2H6(g) –157.3
ethanoic acid (acetic acid) CH3COOH(l) –771.4
ethanol C2H5OH(l) –79.5
ethene (ethylene) C2H4(g) –53.1
ethyne (acetylene) C2H2(g) +11.1
glucose C6H12O6(s) –84.0
hydrogen bromide HBr(g) –484.3
hydrogen chloride HCl(g) –277.6
hydrogen fluoride HF(g) +52.4
hydrogen iodide HI(g) +227.4
hydrogen perchlorate HClO4(l)
hydrogen peroxide H2O2(l) –1 273.3
hydrogen sulfide H2S(g) –36.3
iron(II) oxide FeO(s) –92.3
iron(III) oxide Fe2O3(s) –273.3
iron(II,III) oxide (magnetite) Fe3O4(s) +26.5
lead(II) bromide PbBr2(s) –40.6
lead(II) chloride PbCl2(s) –187.8
lead(II) oxide (red) PbO(s) –20.6
lead(IV) oxide PbO2(s) –272.0
magnesium carbonate MgCO3(s)
MgCl2(s) –824.2
magnesium chloride –1 118.4

–278.7
–359.4
–219.0
–277.4
–1 095.8

–641.3

4

Standard Molar Enthalpies of Formation at 298.15 K cont’d

Name Formula ∆f H° (kJ/mol)

magnesium hydroxide Mg(OH)2(s) – 924.5
magnesium oxide MgO(s) – 601.6
magnesium sulfate – 1 284.9
manganese(II) oxide MgSO4(s) – 385.2
manganese(IV) oxide MnO(s) – 520.0
mercury(II) oxide (red) – 90.8
mercury(II) sulfide (red) MnO2(s)
methanal (formaldehyde) HgO(s) – 58.2
methane – 108.6
methanoic acid (formic acid) HgS(s)
methanol – 74.6
nickel(II) oxide CH2O(g) – 425.0
nitric acid CH4(g) – 239.2
nitrogen dioxide HCOOH(l) – 240.6
nitrogen monoxide – 174.1
octane CH3OH(l)
pentane NiO(s) + 33.2
phosphorus pentachloride + 91.3
phosphorus trichloride (liquid) HNO3(l) – 250.1
phosphorus trichloride (vapour) NO2(g) – 173.5
potassium bromide NO(g) – 443.5
potassium chlorate – 319.7
potassium chloride C8H18(l) – 287.0
potassium hydroxide C5H12(l) – 393.8
propane PCl5(s) – 397.7
silicon dioxide (α-quartz) PCl3(l) – 436.5
silver bromide PCl3(g) – 424.6
silver chloride KBr(s) – 103.8
silver iodide – 910.7
sodium bromide KClO3(s) – 100.4
sodium chloride KCl(s) – 127.0
sodium hydroxide – 61.8
sodium iodide KOH(s) – 361.1
sucrose – 411.2
sulfur dioxide C3H8(g) – 425.8
sulfuric acid SiO2(s) – 287.8
sulfur trioxide (liquid) AgBr(s) – 2 226.1
sulfur trioxide (vapour) – 296.8
tin(II) chloride AgCl(s) – 814.0
tin(IV) chloride – 441.0
tin(II) oxide AgI(s) – 395.7
tin(IV) oxide – 325.1
water (liquid) NaBr(s) – 511.3
water (vapour) – 280.7
zinc oxide NaCl(s) – 577.6
zinc sulfide (sphalerite) – 285.8
NaOH(s) – 241.8
– 350.5
NaI(s) – 206.0

C12H22O11(s)
SO2(g)
H2SO4(l)
SO3(l)
SO3(g)
SnCl2(s)
SnCl4(l)
SnO(s)

SnO2(s)
H2O(l)
H2O(g)
ZnO(s)

ZnS(s)

5

Solubility of Some Common Ionic Compounds in Water at 298.15 K

Ion Group 1 ions F– Cl– CO32– IO3– OH–
NH4+ most Br– SO42– PO43– OOCCOO2–
Solubility NO3– I– SO32–
greater than ClO3– Group 1 ions Group 1 ions Group 1 ions
or equal to ClO4– most most NH4+
0.1 mol/L NH4+ NH4+
(very soluble) CH3COO– most Co(IO3)2
Fe2(OOCCOO)3
most

Solubility RbClO4 Li+ Cu+ Ca2+ most most
CsClO4 Mg2+ Sr2+
less than AgCH3COO Ca2+ Ag+ Ba2+
Hg2(CH3COO)2 Sr2+ Ag+
0.1 mol/L Ba2+ Hg22+ Hg22+
(slightly Fe2+ Pb2+ Pb2+
soluble) Hg22+ Ra2+
Pb2+ Tl+

Note: This solubility table is only a guideline that is established using the Ksp values. A concentration of 0.1 mol/L
corresponds to approximately 10 g/L to 30 g/L depending on molar mass. Hg22+ is a polyatomic ion of mercury.

Flame Colour of Elements

Element Symbol Colour

lithium Li red

sodium Na yellow

potassium K violet

rubidium Rb violet

cesium Cs violet

calcium Ca yellowish red

strontium Sr scarlet red

barium Ba yellowish green

copper Cu blue to green

boron B yellowish green

lead Pb blue-white

Note: The flame test can be used to determine the identity of a metal or a metal ion. Blue to green indicates a range of
colours that might appear.

6

Table of Selected Standard Electrode Potentials*

Reduction Half-Reaction Electrical Potential E° (V)

F2(g) + 2 e– ⇌ 2 F –(aq)...................................................... +2.87
PbO2(s) + SO42–(aq) + 4 H+(aq) + 2 e– ⇌ PbSO4(s) + 2 H2O(l) ................................ +1.69
MnO4–(aq) + 8 H+(aq) + 5 e– ⇌ Mn2+(aq) + 4 H2O(l) ................................ +1.51
Au3+(aq) + 3 e– ⇌ Au(s) ........................................................... +1.50
ClO4–(aq) + 8 H+(aq) + 8 e– ⇌ 2ClC–(la–(qa)q)+...4...H...2..O..(..l.)........................................................................ +1.39
Cl2(g) + 2 e– ⇌ +1.36
2 HNO2(aq) + 4 H+(aq) + 4 e– ⇌ N2O(g) + 3 H2O(l) ................................... +1.30
Cr2O72–(aq) + 14 H+(aq) + 6 e– ⇌ 2 Cr3+(aq) + 7 H2O(l) ............................... +1.23
O2(g) + 4 H+(aq) + 4 e– ⇌ 2 H2O(l) ..................................................... +1.23
MnO2(s) + 4 H+(aq) + 2 e– ⇌ Mn2+(aq) + 2 H2O(l) ................................ +1.22
Br2(l) + 2 e– ⇌ 2 Br–(aq) ..................................................... +1.07
Hg2+(aq) + 2 e– ⇌ Hg(l) ........................................................... + 0.85
OCl–(aq) + H2O(l) + 2 e– ⇌ Cl–(aq) + 2 OH–(aq) ................................. + 0.84
2 NO3–(aq) + 4 H+(aq) + 2 e– ⇌ N2O4(g) + 2 H2O(l) .................................. + 0.80
Ag+(aq) + e– ⇌ Ag(s) ........................................................... + 0.80
Fe3+(aq) + e– ⇌ Fe2+(aq) ...................................................... + 0.77
O2(g) + 2 H+(aq) + 2 e– ⇌ H2O2(l) ....................................................... + 0.70
I2(s) + 2 e– ⇌ 2 I–(aq) ....................................................... + 0.54
O2(g) + C2 uH22+O(a(ql)) + 4 e– ⇌ 4 OH–(aq) ................................................... + 0.40
+ 2 e– ⇌ Cu(s) ........................................................... + 0.34
SO42–(aq) + 4 H+(aq) + 2 e– ⇌ H2SO3(aq) + H2O(l) ................................. + 0.17
Sn4+(aq) + 2 e– ⇌ Sn2+(aq) . .................................................... + 0.15
S(s) + 2 H+(aq) + 2 e– ⇌ H2S(aq) ...................................................... + 0.14
AgBr(s) + e– ⇌ Ag(s) + Br–(aq) ......................................... + 0.07
2 H+(aq) + 2 e– ⇌ H2(g) .......................................................... 0.00
Pb2+(aq) + 2 e– ⇌ Pb(s) ........................................................... – 0.13
Sn2+(aq) + 2 e– ⇌ Sn(s) ........................................................... – 0.14
AgI(s) + e– ⇌ Ag(s) + I–(aq) ........................................... – 0.15
Ni2+(aq) + 2 e– ⇌ Ni(s) ........................................................... – 0.26
Co2+(aq) + 2 e– ⇌ Co(s) ........................................................... – 0.28
PbSO4(s) + 2 e– ⇌ Pb(s) + SO42–(aq) ..................................... – 0.36
Se(s) + 2 H+(aq) + 2 e– ⇌ H2Se(aq) .................................................... – 0.40
Cd2+(aq) + 2 e– ⇌ Cd(s) .......................................................... – 0.40
Cr3+(aq) + e– ⇌ Cr2+(aq) ...................................................... – 0.41
Fe2+(aq) + 2 e– ⇌ Fe(s) ........................................................... – 0.45
NO2–(aq) + H2O(l) + e– ⇌ NO(g) + 2 OH–(aq) .................................. – 0.46
Ag2S(s) + 2 e– ⇌ 2 Ag(s) + S2–(aq) ...................................... – 0.69
Zn2+(aq) + 2 e– ⇌ Zn(s) ........................................................... – 0.76
2 H2O(l) + 2 e– ⇌ H2(g) + 2OH–(aq) .................................... – 0.83
Cr2+(aq) + 2 e– ⇌ Cr(s) ........................................................... – 0.91
Se(s) + 2 e– ⇌ Se2–(aq) ...................................................... – 0.92
SO42–(aq) +AHl32+O(a(ql)) + 2 e– ⇌ SO32–(aq) + 2OH–(aq) ............................. – 0.93
+ 3 e– ⇌ Al(s) ........................................................... –1.66
Mg2+(aq) + 2 e– ⇌ Mg(s) .......................................................... –2.37
Na+(aq) + e– ⇌ Na(s) ........................................................... –2.71
Ca2+(aq) + 2 e– ⇌ Ca(s) ........................................................... –2.87
Ba2+(aq) + 2 e– ⇌ Ba(s) ........................................................... –2.91
K+(aq) + e– ⇌ K(s) ............................................................. –2.93
Li+(aq) + e– ⇌ Li(s)............................................................. –3.04

*For 1.0 mol/L solutions at 298.15 K (25.00 °C) and a pressure of 101.325 kPa
7

Relative Strengths of Acids and Bases at 298.15 K

Common Name Acid Formula Conjugate Base Formula Ka
IUPAC / Systematic Name very large
very large
perchloric acid HClO4(aq) ClO4–(aq) very large
aqueous hydrogen perchlorate HI(aq) I –(aq) very large
hydroiodic acid HBr(aq) Br–(aq) very large
aqueous hydrogen iodide HCl(aq) Cl–(aq) very large
hydrobromic acid H2SO4(aq) HSO4–(aq)
aqueous hydrogen bromide HNO3(aq) NO3–(aq) 1
hydrochloric acid 5.6 × 10 –2
aqueous hydrogen chloride 1.4 × 10 –2
sulfuric acid 1.0 × 10 –2
aqueous hydrogen sulfate 6.9 × 10 –3
nitric acid 7.4 × 10 – 4
aqueous hydrogen nitrate 6.3 × 10 – 4
5.6 × 10 – 4
hydronium ion H3O+(aq) H2O(l) 1.8 × 10 – 4
1.5 × 10 – 4
oxalic acid HOOCCOOH(aq) HOOCCOO–(aq) 1.4 × 10 – 4
9.1 × 10 –5
8 sulfurous acid H2SO3(aq) HSO3–(aq)
aqueous hydrogen sulfite HSO4–(aq) SO42–(aq)
H3PO4(aq) H2PO4–(aq)
hydrogen sulfate ion C3H5O(COOH)3(aq) C3H5O(COOH)2COO–(aq)
HF(aq) F–(aq)
phosphoric acid HNO2(aq) NO2–(aq)
aqueous hydrogen phosphate HCOOH(aq) HCOO–(aq)
citric acid HOOCCOO–(aq) OOCCOO2–(aq)
2-hydroxy-1,2,3-propanetricarboxylic acid
hydrofluoric acid
aqueous hydrogen fluoride
nitrous acid
aqueous hydrogen nitrite
formic acid
methanoic acid

hydrogen oxalate ion

lactic acid C2H5OCOOH(aq) C2H5OCOO–(aq)
2-hydroxypropanoic acid HC6H6O6–(aq)

ascorbic acid H2C6H6O6(aq)
2(1,2-dihydroxyethyl)-4,5-dihydroxy-furan-3-one

benzoic acid C6H5COOH(aq) C6H5COO–(aq) 6.3 × 10 –5
benzenecarboxylic acid CH3COOH(aq) CH3COO–(aq) 1.8 × 10 –5
acetic acid C3H5O(COOH)2COO–(aq) C3H5OCOOH(COO)22–(aq) 1.7 × 10 –5
ethanoic acid

dihydrogen citrate ion

butanoic acid C3H7COOH(aq) C3H7COO–(aq) 1.5 × 10 –5

propanoic acid C2H5COOH(aq) C2H5COO–(aq) 1.3 × 10 –5
carbonic acid (CO2 + H2O) 4.5 × 10 –7
aqueous hydrogen carbonate H2CO3(aq) HCO3–(aq) 4.0 × 10 –7
hydrogen citrate ion 8.9 × 10 – 8
hydrosulfuric acid C3H5OCOOH(COO)22–(aq) C3H5O(COO)33–(aq) 6.3 × 10 – 8
aqueous hydrogen sulfide
hydrogen sulfite ion H2S(aq) HS–(aq)

HSO3–(aq) SO32–(aq)

9 dihydrogen phosphate ion H2PO4–(aq) HPO42–(aq) 6.2 × 10 – 8
HOCl(aq) OCl–(aq) 4.0 × 10 – 8
hypochlorous acid HCN(aq) CN–(aq) 6.2 × 10 –10
aqueous hydrogen hypochlorite NH4+(aq) NH3(aq) 5.6 × 10 –10
hydrocyanic acid
aqueous hydrogen cyanide

ammonium ion

hydrogen carbonate ion HCO3–(aq) CO32–(aq) 4.7 × 10 –11

hydrogen ascorbate ion HC6H6O6–(aq) C6H6O62–(aq) 2.0 × 10 –12

hydrogen phosphate ion HPO42–(aq) PO43–(aq) 4.8 × 10 –13

water H2O(l) OH –(aq) 1.0 × 10 –14

Note: An approximation may be used instead of the quadratic formula when the concentration of H3O+ produced is less than 5% of the original acid
concentration (or the concentration of the acid is 1 000 times greater than the Ka). An approximation can also be used for weak bases. The formulas
of the carboxylic acids have been written so that the COOH group can be easily recognized. Either the common or IUPAC name is acceptable.

Acid–Base Indicators at 298.15 K

Indicator Suggested pH Range Colour Change as Ka
methyl violet Abbreviations pH Increases
cresol red ~2 × 10 –1
thymol blue HMv(aq) / Mv–(aq) 0.0 – 1.6 yellow to blue
orange IV ~3 × 10 –1
H2Cr(aq) / HCr–(aq) 0.0 – 1.0 red to yellow 3.5 × 10 –9
HCr–(aq) / Cr2–(aq) 7.0 – 8.8 yellow to red 2.2 × 10 –2
H2Tb(aq) / HTb–(aq) 1.2 – 2.8 red to yellow 6.3 × 10 –10
HTb–(aq) / Tb2–(aq) 8.0 – 9.6 yellow to blue
~1 × 10 –2
HOr(aq) / Or–(aq) 1.4 – 2.8 red to yellow

methyl orange HMo(aq) / Mo–(aq) 3.2 – 4.4 red to yellow 3.5 × 10 –4

bromocresol green HBg(aq) / Bg–(aq) 3.8 – 5.4 yellow to blue 1.3 × 10 –5

methyl red HMr(aq) / Mr–(aq) 4.8 – 6.0 red to yellow 1.0 × 10 –5

chlorophenol red HCh(aq) / Ch–(aq) 5.2 – 6.8 yellow to red 5.6 × 10 –7

bromothymol blue HBb(aq) / Bb–(aq) 6.0 – 7.6 yellow to blue 5.0 × 10 –8

phenol red HPr(aq) / Pr–(aq) 6.6 – 8.0 yellow to red 1.0 × 10 –8

phenolphthalein HPh(aq) / Ph–(aq) 8.2 – 10.0 colourless to pink 3.2 × 10 –10

thymolphthalein HTh(aq) / Th–(aq) 9.4 – 10.6 colourless to blue 1.0 × 10 –10

alizarin yellow R HAy(aq) / Ay–(aq) 10.1 – 12.0 yellow to red 6.9 × 10 –12

indigo carmine HIc(aq) / Ic–(aq) 11.4 – 13.0 blue to yellow ~6 × 10 –12
12.0 – 14.0 ~1 × 10 –13
1,3,5–trinitrobenzene HNb(aq) / Nb–(aq) colourless
to orange

10

Colours of Common Aqueous Ions

Solution Concentration

Ionic Species 1.0 mol/L 0.010 mol/L

chromate yellow pale yellow

chromium(III) blue-green green

chromium(II) dark blue pale blue

cobalt(II) red pink

copper(I) blue-green pale blue-green

copper(II) blue pale blue

dichromate orange pale orange

iron(II) lime green colourless

iron(III) orange-yellow pale yellow

manganese(II) pale pink colourless

nickel(II) blue-green pale blue-green

permanganate deep purple purple-pink

11

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