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Home , Solubility table

Data Booklet Updated 2010 1 2 3 4 5 6 7 8 9

Table of Common Polyatomic Ions

acetate (ethanoate) CH COO – chromate Cr O 2 – phosphate PO 3 – 1 1.01 3 4 4 1+,1– + 2 – 2 – ammonium NH4 dichromate Cr2O7 hydrogen phosphate HPO4 2.2 – – – benzoate C6H5COO cyanide CN dihydrogen phosphate H2PO4

3 – – 2 – H borate BO3 hydroxide OH silicate SiO3 hydrogen 2 – – 2 – carbide C2 iodate IO3 sulfate SO4 3 6.94 4 9.01 carbonate CO 2 – nitrate NO – hydrogen sulfate HSO – 1+ 2+ 3 3 4 – – 2 – 1.0 1.6 hydrogen carbonate HCO3 nitrite NO2 sulfite SO3 – 2 – – perchlorate CIO4 OOCCOO hydrogen sulfite HSO3 Li Be – – – CIO hydrogen oxalate HOOCCOO HS lithium beryllium 3 chlorite CIO – permanganate MnO – thiocyanate SCN – 11 22.99 12 24.31 2 4 – – 2 – 2 – 1+ 2+ hypochlorite OCl or CIO peroxide O2 thiosulfate S2O3

0.9 1.3 2 – persulfide S2 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 58 140.12 59 140.91 60 144.24 61 (145) 62 150.36 3+ 3+ 3+ 3+ 3+, 2+ References 1.1 1.1 1.1 — 1.2 Lide, D.R. 2005. CRC Handbook of Chemistry and Physics. 86th ed. Boca Raton: CRC Press. Ce Pr Nd Pm Sm cerium praseodymium neodymium promethium samarium Speight, James G. 2005. Lange’s Handbook of Chemistry. 16th ed. New York: McGraw-Hill, Inc. 90 232.04 91 231.04 92 238.03 93 (237) 94 (244) 4+ 5+, 4+ 6+, 4+ 5+ 4+, 6+ IUPAC commission on atomic weights and 1.3 1.5 1.7 1.3 1.3 isotopic abundances. 2002. http://www.chem. qmw.ac.uk/iupac/AtWt/index.html. 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 — — Note: The legend denotes the physical state of the elements Key Atomic molar at exactly 101.325 kPa and 298.15 K. He mass (g/mol)* Atomic number 26 55.85 Most stable 3+, 2+ ion charges 5 10.81 6 12.01 7 14.01 8 16.00 9 19.00 10 20.18 Electronegativity 1.8 — — — — — — 2.0 2.6 3.0 3.4 4.0 — Symbol Fe Name iron B C N O F Ne boron carbon nitrogen fluorine neon

12 14 28.09 15 30.97 16 32.07 17 35.45 18 39.95 * Based on 6 C 13 26.98 — 3+ — — — — ( ) Indicates mass of the most stable isotope 1.6 1.9 2.2 2.6 3.2 —

Al Si P S Cl Ar aluminium silicon phosphorus sulfur chlorine 58.69 63.55 65.41 69.72 72.64 33 74.92 34 78.96 35 79.90 36 83.80 28 29 30 31 32 — — — — 2+, 3+ 2+, 1+ 2+ 3+ 4+ 2.2 2.6 3.0 — 1.9 1.9 1.7 1.8 2.0

Ni Cu Zn Ga Ge As Se Br Kr nickel copper zinc gallium germanium arsenic selenium bromine krypton 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 1.7 1.8 2.0 2.1

Pd Ag Cd In Sn Sb Te I Xe palladium silver cadmium indium tin antimony tellurium iodine xenon ( ) 85 (210) 86 (222) 78 195.08 79 196.97 80 200.59 81 204.38 82 207.2* 83 208.98 84 209 — 4+, 2+ 3+, 1+ 2+, 1+ 1+, 3+ 2+, 4+ 3+, 5+ 2+, 4+ — 2.2 — 2.2 2.4 1.9 1.8 1.8 1.9 2.0 902 254 Pt Au Hg Tl Pb Bi Po At Rn 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+ — — — — — — — — —

Am Cm Bk Cf Es 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 kJ/mol I current A or C/s

Kc equilibrium constant —

Ka acid ionization (dissociation) constant —

Kb base ionization (dissociation) constant — M molar mass g/mol m mass g n amount of substance mol P kPa Q charge C T (absolute) K t temperature (Celsius) °C t time s V volume L c amount 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) –14 Kw = 1.0 × 10 at 298.15 K (for ion in mol/L)

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

Quadratic Formula

2 x = --bb! 4ac 2a

Selected SI Prefixes

Exponential Prefix Symbol Value tera T 1012 giga G 109 mega M 106 kilo k 103 milli m 10 –3 micro µ 10 –6 nano n 10 –9 pico 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 NH3(g) –45.9 NH4Cl(s) –314.4 NH4NO3(s) –365.6 BaCO3(s) –1 213.0 BaCl2(s) –855.0 Ba(OH)2(s) –944.7 BaO(s) –548.0 BaSO4(s) –1 473.2 benzene C6H6(l) +49.1 butane C4H10(g) –125.7 CaCO3(s) –1 207.6 CaCl2(s) –795.4 Ca(OH)2(s) –985.2 CaO(s) –634.9 CaSO4(s) –1 434.5 CO2(g) –393.5 CO(g) –110.5 chromium(III) oxide Cr2O3(s) –1 139.7 copper(I) oxide Cu2O(s) –168.6 copper(II) oxide CuO(s) –157.3 copper(II) sulfate CuSO4(s) –771.4 copper(I) sulfide Cu2S(s) –79.5 copper(II) sulfide CuS(s) –53.1 dinitrogen tetroxide N2O4(g) +11.1 ethane C2H6(g) –84.0 ethanoic acid (acetic acid) CH3COOH(l) –484.3 ethanol C2H5OH(l) –277.6 ethene (ethylene) C2H4(g) +52.4 ethyne (acetylene) C2H2(g) +227.4 C6H12O6(s) –1 273.3 hydrogen bromide HBr(g) –36.3 HCl(g) –92.3 hydrogen fluoride HF(g) –273.3 hydrogen iodide HI(g) +26.5 hydrogen perchlorate HClO4(l) –40.6 hydrogen peroxide H2O2(l) –187.8 hydrogen sulfide H2S(g) –20.6 iron(II) oxide FeO(s) –272.0 iron(III) oxide Fe2O3(s) –824.2 iron(II,III) oxide (magnetite) Fe3O4(s) –1 118.4 lead(II) bromide PbBr2(s) –278.7 lead(II) chloride PbCl2(s) –359.4 lead(II) oxide (red) PbO(s) –219.0 lead(IV) oxide PbO2(s) –277.4 MgCO3(s) –1 095.8 MgCl2(s) –641.3

4 Standard Molar Enthalpies of Formation at 298.15 K cont’d

Name Formula ∆f H° (kJ/mol) Mg(OH)2(s) – 924.5 MgO(s) – 601.6 MgSO4(s) – 1 284.9 manganese(II) oxide MnO(s) – 385.2 manganese(IV) oxide MnO2(s) – 520.0 mercury(II) oxide (red) HgO(s) – 90.8 mercury(II) sulfide (red) HgS(s) – 58.2 methanal (formaldehyde) CH2O(g) – 108.6 methane CH4(g) – 74.6 methanoic acid (formic acid) HCOOH(l) – 425.0 methanol CH3OH(l) – 239.2 nickel(II) oxide NiO(s) – 240.6 nitric acid HNO3(l) – 174.1 nitrogen dioxide NO2(g) + 33.2 nitrogen monoxide NO(g) + 91.3 octane C8H18(l) – 250.1 pentane C5H12(l) – 173.5 phosphorus pentachloride PCl5(s) – 443.5 phosphorus trichloride (liquid) PCl3(l) – 319.7 phosphorus trichloride (vapour) PCl3(g) – 287.0 KBr(s) – 393.8 KClO3(s) – 397.7 KCl(s) – 436.5 KOH(s) – 424.6 propane C3H8(g) – 103.8 (α-quartz) SiO2(s) – 910.7 AgBr(s) – 100.4 AgCl(s) – 127.0 silver iodide AgI(s) – 61.8 NaBr(s) – 361.1 NaCl(s) – 411.2 NaOH(s) – 425.8 NaI(s) – 287.8 C12H22O11(s) – 2 226.1 SO2(g) – 296.8 sulfuric acid H2SO4(l) – 814.0 sulfur trioxide (liquid) SO3(l) – 441.0 sulfur trioxide (vapour) SO3(g) – 395.7 tin(II) chloride SnCl2(s) – 325.1 tin(IV) chloride SnCl4(l) – 511.3 tin(II) oxide SnO(s) – 280.7 tin(IV) oxide SnO2(s) – 577.6 water (liquid) H2O(l) – 285.8 water (vapour) H2O(g) – 241.8 ZnO(s) – 350.5 zinc sulfide (sphalerite) ZnS(s) – 206.0

5 of Some Common Ionic Compounds in Water at 298.15 K

Group 1 ions NH + 4 Cl– CO 2– – 3 – NO3 – – 2– 3– IO3 – Ion F Br SO4 PO4 OH ClO – OOCCOO2– 3 I– SO 2– – 3 ClO4 – CH3COO

Solubility Group 1 ions Group 1 ions Group 1 ions greater than NH + or equal to most most most most 4 NH + NH + 0.1 mol/L 4 Co(IO3)2 4

(very soluble) Fe2(OOCCOO)3

Li+ Ca2+ Mg2+ Cu+ Sr2+ Solubility 2+ RbClO4 Ca + 2+ less than 2+ Ag Ba CsClO4 Sr 2+ + 0.1 mol/L 2+ Hg2 Ag most most most (slightly AgCH3COO Ba 2+ 2+ Pb Hg2 soluble) Hg (CH COO) Fe2+ 2 3 2 Tl+ Pb2+ Hg 2+ 2 Ra2+ Pb2+

Note: This solubility table is only a guideline that is established using the Ksp values. A concentration of 0.1 mol/L 2+ corresponds to approximately 10 g/L to 30 g/L depending on molar mass. Hg2 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 2F (aq)...... +2.87 2– + – PbO2(s) + SO4 (aq) + 4 H (aq) + 2 e PbSO4(s) + 2 H2O(l) ...... +1.69 – + – ⇌ 2+ MnO4 (aq) + 8 H (aq) + 5 e Mn (aq) + 4 H2O(l) ...... +1.51 Au3+(aq) + 3 e– ⇌ Au(s) ...... +1.50 – + – ⇌ – ClO4 (aq) + 8 H (aq) + 8 e Cl (aq) + 4 H2O(l) ...... +1.39 – ⇌ – Cl2(g) + 2 e 2 Cl (aq) ...... +1.36 + – ⇌ 2 HNO2(aq) + 4 H (aq) + 4 e N2O(g) + 3 H2O(l) ...... +1.30 2– + – ⇌ 3+ Cr2O7 (aq) + 14 H (aq) + 6 e 2 Cr (aq) + 7 H2O(l) ...... +1.23 + – ⇌ O2(g) + 4 H (aq) + 4 e 2H2O(l) ...... +1.23 + – ⇌ 2+ MnO2(s) + 4 H (aq) + 2 e Mn (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 2I (aq) ...... +0.54 – ⇌ – O2(g) + 2 H2O(l) + 4 e 4 OH (aq) ...... +0.40 Cu2+(aq) + 2 e– ⇌ Cu(s) ...... +0.34 2– + – ⇌ SO4 (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 + – 2H (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 – ⇌ 2– PbSO4(s) + 2 e Pb(s) + SO4 (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 – ⇌ 2– Ag2S(s) + 2 e 2 Ag(s) + S (aq) ...... – 0.69 Zn2+(aq) + 2 e– ⇌ Zn(s) ...... – 0.76 – ⇌ – 2H2O(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 2– – ⇌ 2– – SO4 (aq) + H2O(l) + 2 e SO3 (aq) + 2OH (aq) ...... – 0.93 Al3+(aq) + 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 at 298.15 K (25.00 °C) ⇌and a pressure of 101.325 kPa 7 –3 –5 –2 –2 –2 –4 –4 –4 –4 –4 –4 a

1 K × 10 × 10 × 10 × 10 × 10 × 10 very large very very large very very large very very large very very large very very large very 9.1 1.0 1.4 5.6 7.4 × 10 7.4 6.9 × 10 6.9 1.4 1.8 × 10 1.8 5.6 1.5 × 10 1.5 6.3 × 10 6.3 (aq) – COO 2

(aq) (aq) (aq) – (aq) (aq) – (aq) (aq) 2– – 6 (aq) (aq) (aq) (aq) – O – (aq) (aq) (aq) (aq) (aq) (aq) 6 (aq) (aq) 4 – – (aq) (aq) (aq) (aq) OCOO O(COOH) – 4 3 – – 5 5 H 4 2– 2 3 (aq) (aq) 6 (aq) (aq) 4 PO O(l) O(l) H H – (aq) (aq) – (aq) (aq) 2 2 2 3 – – Conjugate Base Formula Base Conjugate I Br Cl F HCOO HOOCCOO HSO HC H ClO NO SO HSO NO C OOCCOO C H (aq) 3

(aq) (aq) – (aq) (aq) 6 O 6 (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) Acid Formula Acid (aq) (aq) (aq) (aq) – 4 4 4 3 (aq) (aq) 2 3 H OCOOH(aq) O(COOH) 4 + 5 6 5 SO SO C O PO H H 2 2 2 3 3 2 3 H HI(aq) HI(aq) HBr(aq) HBr(aq) HCl(aq) HCl(aq) H HClO H HSO H C HF(aq) HNO HCOOH(aq) HOOCCOO C H HOOCCOOH(aq) HOOCCOOH(aq) HNO Relative Strengths of Acids and Bases at 298.15 K 298.15 at Bases and Acids of Strengths Relative Name Common IUPAC / Systematic Name / Systematic IUPAC sulfuric acid sulfate hydrogen aqueous acid hydroiodic iodide hydrogen aqueous acid hydrobromic bromide hydrogen aqueous acid hydrochloric chloride hydrogen aqueous hydronium ion hydronium acid perchloric perchlorate hydrogen aqueous sulfurous acid sulfite hydrogen aqueous ion sulfate hydrogen acid phosphoric phosphate hydrogen aqueous acid citric acid 2-hydroxy-1,2,3-propanetricarboxylic acid hydrofluoric fluoride hydrogen aqueous acid nitrous nitrite hydrogen aqueous acid formic acid methanoic ion oxalate hydrogen acid lactic acid 2-hydroxypropanoic acid ascorbic 2(1,2-dihydroxyethyl)-4,5-dihydroxy-furan-3-one oxalic nitric acid nitrate hydrogen aqueous

8 –7 –7 –5 –5 –5 –5 –5 –8 –8 –8 –8 – 11 –14 –10 –10 –13 –12 × 10 × 10 × 10 × 10 × 10 × 10 × 10 1.7 1.8 × 10 1.8 1.3 × 10 1.3 4.0 1.5 × 10 1.5 4.5 × 10 4.5 6.3 × 10 6.3 8.9 4.0 6.2 × 10 6.2 6.3 × 10 6.3 4.7 1.0 5.6 4.8 × 10 4.8 6.2 × 10 6.2 × 10 2.0 (aq) 2– 2 (aq) 3– 3 (aq) (aq) (aq) (aq) (aq) (aq) – – – (aq) – produced is less than 5% of the original of than acid less is 5% produced 2– (aq) (aq) + (aq) (aq) 6 (aq) (aq) – (aq) (aq) (aq) (aq) 2– O COO COO O O(COO) OCOOH(COO) COO (aq) (aq) 3 4 (aq) (aq) (aq) (aq) (aq) 3 5 COO 5 5 5 6 7 2– (aq) (aq) – 3– 2– – 3 – 3 3 4 – 3 H H H H H H 2 6 3 3 3 6 OCl CN C NH CO C HS PO SO CH C C HPO OH C C HCO (aq) (aq) ). An approximation can also be used for weak bases. The formulas The formulas bases. weak can also be An used for approximation ). – a 2– 2 COO 2 (aq) – 6 (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) O – (aq) (aq) – 3 6 4 2– – (aq) (aq) COOH(aq) COOH(aq) COOH(aq) OCOOH(COO) O(COOH) COOH(aq) 3 4 3 + 5 COOH(aq) COOH(aq) 5 5 5 H 7 4 3 6 S(aq) S(aq) PO CO O(l) H H H H H 2 2 2 2 2 6 3 3 3 C CH C C C C H HSO H HOCl(aq) HCN(aq) NH HCO HC HPO H H

O) 2 + H 2 acid benzoic acid benzenecarboxylic acid acetic acid ethanoic ion citrate dihydrogen acid butanoic acid propanoic (CO carbonic acid ion citrate hydrogen acid hydrosulfuric sulfide hydrogen aqueous ion sulfite hydrogen ion phosphate dihydrogen acid hypochlorous hypochlorite hydrogen aqueous acid hydrocyanic cyanide hydrogen aqueous ammonium ion carbonate ion hydrogen ion ascorbate hydrogen ion phosphate hydrogen water aqueous hydrogen carbonate hydrogen aqueous concentration (or the concentration of the acid is 1 000 is the acid of times the greater concentration than the K (or concentration An approximation may be used instead of the quadratic formula when the concentration of H of the concentration when the be used insteadquadratic of formula may An approximation of the carboxylic acids have been written so that the COOH group can be easily recognized. Either the common or IUPAC name is acceptable. name acceptable. is been written canrecognized. that group so the be IUPAC the easily COOH or common Either have acids the carboxylic of Note:

9 Acid–Base Indicators at 298.15 K

Suggested Colour Change as Indicator Abbreviations pH Range pH Increases Ka methyl violet HMv(aq) / Mv–(aq) 0.0 – 1.6 yellow to blue ~2 × 10 –1

H Cr(aq) / HCr–(aq) 0.0 – 1.0 red to yellow ~3 × 10 –1 cresol red 2 HCr–(aq) / Cr2–(aq) 7.0 – 8.8 yellow to red 3.5 × 10 –9

H Tb(aq) / HTb–(aq) 1.2 – 2.8 red to yellow 2.2 × 10 –2 thymol blue 2 HTb–(aq) / Tb2–(aq) 8.0 – 9.6 yellow to blue 6.3 × 10 –10 orange IV HOr(aq) / Or–(aq) 1.4 – 2.8 red to yellow ~1 × 10 –2 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 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

colourless 1,3,5–trinitrobenzene HNb(aq) / Nb–(aq) 12.0 – 14.0 ~1 × 10 –13 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 Notes: ......

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