Table of substances solubility by temperature
Table shows solubility of various substances under different temperature given in grams of dissoluted substance per 100g of water.

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# other inorganic

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C ammonia NH3 90 53 31 - - -

# gases

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C ammonia NH3 90 53 31 - - - nitrogen N2 0.2914 0.1922 0.1463 0.1265 0.119 0.1178 carbon dioxide CO2 0.3346 0.1688 0.0973 0.0576 - - hydrogen chloride HCl 82.3 72 63.3 56.1 - - hydrogen sulfuride H2S - 0.385 - - - - ethyne C2H2 - 0.117 - - - - nitrogen (II) oxide NO - 0.0056 - - - - nitrogen (I) oxide N2O - 0.112 - - - - chlorine Cl2 4.61 2.23 1.44 1.02 0.68 - hydrogen H2 0.0192 0.0162 0.0146 0.0143 0.0143 0.0143 oxygen O2 0.6993 0.4433 0.3303 0.2789 0.2517 0.246

# oxides

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C carbon dioxide CO2 0.3346 0.1688 0.0973 0.0576 - - carbon monoxide CO 0.035 0.023 0.018 0.015 0.014 0.014 nitrogen (II) oxide NO - 0.0056 - - - - nitrogen (I) oxide N2O - 0.112 - - - -

# salts

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C potassium bromide KBr 53.5 65.2 75.5 85.5 95 104 potassium chloride KCl 27.6 34 40 45.5 51.1 56.7 potassium jodide KI 127.5 144 160 176 192 208 silver chloride AgCl - 0.00015 - - - - potassium chromate K2CrO4 58.2 61.7 65.2 68.6 72.1 75.6 silver iodide AgI - - - 0.000003 - - silver (I) sulfate (VI) Ag2SO4 0.57 0.79 0.97 1.14 1.28 1.39 barium chromate (VI) BaCrO4 0.0002 0.00037 - - - - barium sulfate (VI) BaSO4 0.000115 0.00024 - - - 0.000413 mercury (I) chloride Hg2Cl2 0.00014 0.0002 - - - - mercury (II) chloride HgCl2 3.5 6.1 9.3 14 23.1 38 silver nitrate (V) AgNO3 122 222 376 525 669 952 aluminium sulfate (VI) Al2(SO4)3 23.8 26.7 31.4 37.2 42.2 47.1 barium chloride BaCl2 31.6 35.7 40.7 46.4 52.4 58.8 barium nitrate (III) Ba(NO3)2 5 9.2 14.2 20.3 27 34.2 potassium thiocyanate KSCN 63.9 68.5 - - - - potassium nitrate (III) KNO2 73.6 74.9 77 - - 80.5 potassium nitrate (V) KNO3 13.3 31.6 63.9 110 169 246 sodium nitrate (V) NaNO3 73 88 104 124 148 180 potassium sulfate (VI) K2SO4 7.35 11.11 14.76 18.17 21.75 24.1 ammonium thiocyanate NH4SCN 54.5 63 - - - - ammonium oxalate (NH4)2C2O4 2.1 4.2 9.3 - - - ammonium chloride NH4Cl 29.4 37.2 45.8 55.2 65.6 77.3 ammonium magnesium phosphate NH4MgPO4 0.023 0.052 0.036 0.04 0.019 - ammonium nitrate (V) NH4NO3 118.3 192 297 421 580 871 lead (II) nitrate (V) Pb(NO3)2 38.8 56.3 75 96 115 138.8 ammonium sulfate (VI) (NH4)2SO4 70.6 75.4 81 88 95.3 103.3 sodium chloride NaCl 35.7 36 36.6 37.3 38.4 39.8

# inorganic acids

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C hydrogen chloride HCl 82.3 72 63.3 56.1 - - hydrogen sulfuride H2S - 0.385 - - - -

# hydrocarbons

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C ethyne C2H2 - 0.117 - - - -

# hydroxides

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C calcium hydroxide Ca(OH)2 0.185 0.165 0.141 0.116 0.094 0.077 barium hydroxide Ba(OH)2 1.67 3.89 8.22 20.94 101.4 -

# halogens

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C chlorine Cl2 4.61 2.23 1.44 1.02 0.68 - bromine Br2 4.22 3.2 - - - - jodine I2 - 0.029 0.056 - - -

# liquids

 Substance Molecular formula 0 °C 20 °C 40 °C 60 °C 80 °C 100 °C bromine Br2 4.22 3.2 - - - -

# Some facts

• Solubility is the ability of one chemical substance to dissolve in another one called solvent.
• As a result of dissolution, a homogeneous solution is formed.
• Depending on the needs, many different units of solubility are used, e.g.:
• grams per 100 grams of solvent (g / 100 g),
• grams per 1 kilogram of solvent (g / 1 kg),
• grams per 100 cm3 of solvent (g / 100 cm3),
• grams per litre of solvent, (g/l),
• moles per litre of solvent (n/l),
• etc.
• The solubility for a specific substances pair (solvent and dissoluted substance) depends on many factors. Among others, these are:
• kind of dissolved substance,
• kind of solvent,
• temperature,
• pressure,
• concentration of common ions in solution,
• complexation,
• the ion strength of the solution,
• crystal size,
• etc.
• The solubility of gases is inversely proportional to temperature, i.e. it decreases with temperature.
• At a constant temperature, the solubility of gases is met by Henry's law:
$c = k \times p$
where:
• c - gas concentration in the liquid,
• k - proportionality coefficient specific for selected gas, solubility and temperature,
• p - partial pressure of gas.