Solubility chart

A solubility chart is a chart with a list of ions and how, when mixed with other ions, they can become precipitates or remain aqueous.

The following chart shows the solubility of multiple independent and various compounds, in water, at a pressure of 1 atm and at room temperature (approx. 293.15 K). Any box that reads "soluble" results in an aqueous product in which no precipitate has formed, while "slightly soluble" and "insoluble" markings mean that there is a precipitate that will form (usually, this is a solid), however, "slightly soluble" compounds such as calcium sulfate may require heat to form its precipitate. Boxes marked "other" can mean that many different states of products can result. For more detailed information of the exact solubility of the compounds, see the solubility table.

The chemicals have to be exposed to their boiling point to fully dissolve.

Note: All the dichromates are water-soluble. In a base, dichromates convert into chromates and some of the chromates are insoluble in water.

  Fluoride
F−		 Chloride
Cl−		 Bromide
Br−		 Iodide
I−		 Carbonate
CO32−		 Chlorate
ClO3−		 Hydroxide
OH−		 Cyanide
CN−		 Cyanate
OCN−		 Thiocyanate
SCN−		 Nitrate
NO3−		 Oxide
O2−		 Phosphate
PO43−		 Sulfate
SO42−		 Dichromate
Cr2O72−[1]
Lithium
Li+		 sS S S S sS S S S ? S S R I S S
Sodium
Na+		 S S S S S S S S S S S R S S S
Potassium
K+		 S S S S S S S S S S S R S S S
Ammonium
NH4+[lower-alpha 1]		 S S S S S S S S ? S S ? S S S
Beryllium
Be2+		 S S S R ? ? ? ? ? ? S R ? S ?
Magnesium
Mg2+		 sS S S S I S I ? ? ? S I I S S
Calcium
Ca2+		 I S S S I S sS S ? ? S R I sS S
Strontium
Sr2+		 sS S S S I S S ? ? ? S R ? I ?
Barium
Ba2+		 sS S S S I S S S ? ? S R I[2] I ?
Zinc
Zn2+		 sS S S S I S I I ? ? S I I S S
Iron(II)
Fe2+		 S S S S I S I ? ? ? S I I S S
Copper(II)
Cu2+		 sS S S ? I S I ? ? I S I I S S
Aluminium
Al3+		 S S S S (partial electrolysis) ? S I ? ? ? S I I S S
Iron(III)
Fe3+		 X[lower-alpha 2] S S ? X S I ? ? ? S I I sS S
Lead(II)
Pb2+		 sS sS sS I I S I ? ? sS S I I I ?
Silver
Ag+		 S I I I I S sS I I sS S sS I sS S
  Fluoride
F−		 Chloride
Cl−		 Bromide
Br−		 Iodide
I−		 Carbonate
CO32−[lower-alpha 1]		 Chlorate
ClO3−[lower-alpha 1]		 Hydroxide
OH−		 Cyanide
CN−		 Cyanate
OCN−		 Thiocyanate
SCN−		 Nitrate
NO3−[lower-alpha 1]		 Oxide
O2−		 Phosphate
PO43−		 Sulfate
SO42−		 Dichromate
Cr2O72−
Key:
Ssoluble
Iinsoluble
sSslightly soluble
Xother
Rreacts with water
?unavailable

See also
  • Solubility rules

Notes
  1. Compounds that include ammonium (NH4+), chlorate (ClO3−), or nitrate (NO3−) are soluble without exceptions. Compounds that include carbonate (CO32−) are insoluble, unless the compound includes group IA elements or ammonium.[3]
  2. Anhydrous FeF3 is slightly soluble in water, FeF3·3H2O is much more soluble in water.

References
  1. "Chromate and dichromate", Wikipedia, 2019-09-25, retrieved 2019-11-25
  2. Hazen, Jeffery L.; Cleary, David A. (July 2, 2014). "Yielding Unexpected Results: Precipitation of Ba3(PO4)2 and Implications for Teaching Solubility Principles in the General Chemistry Curriculum". Journal of Chemical Education. 91 (8): 1261–1263. doi:10.1021/ed400741k.
  3. "Solubility Table". intro.chem.okstate.edu.
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