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 CO3^2−	Chlorate ClO3^−	Hydroxide OH^−	Cyanide CN^−	Cyanate OCN^−	Thiocyanate SCN^−	Nitrate NO3^−	Oxide O^2−	Phosphate PO4^3−	Sulfate SO4^2−	Dichromate Cr2O7^2−[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 Be^2+	S	S	S	R	I	?	?	?	?	?	S	R	?	S	?
Magnesium Mg^2+	sS	S	S	S	I	S	I	?	?	?	S	I	I	S	S
Calcium Ca^2+	I	S	S	S	I	S	sS	S	?	?	S	R	I	sS	S
Strontium Sr^2+	sS	S	S	S	I	S	S	?	?	?	S	R	?	I	?
Barium Ba^2+	sS	S	S	S	I	S	S	S	?	?	S	R	I[2]	I	?
Zinc Zn^2+	sS	S	S	S	I	S	I	I	?	?	S	I	I	S	S
Iron(II) Fe^2+	S	S	S	S	I	S	I	?	?	?	S	I	I	S	S
Copper(II) Cu^2+	sS	S	S	?	I	S	I	?	?	I	S	I	I	S	S
Aluminium Al^3+	S	S	S	S (partial electrolysis)	?	S	I	?	?	?	S	I	I	S	S
Iron(III) Fe^3+	X[lower-alpha 2]	S	S	?	X	S	I	?	?	?	S	I	I	sS	S
Lead(II) Pb^2+	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 CO3^2−[lower-alpha 1]	Chlorate ClO3^−[lower-alpha 1]	Hydroxide OH^−	Cyanide CN^−	Cyanate OCN^−	Thiocyanate SCN^−	Nitrate NO3^−[lower-alpha 1]	Oxide O^2−	Phosphate PO4^3−	Sulfate SO4^2−	Dichromate Cr2O7^2−

Key:

S	soluble
I	insoluble
sS	slightly soluble
X	other
R	reacts 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.