Solubility chart

Chart describing whether ionic compounds dissolve or precipitate From Wikipedia, the free encyclopedia

A solubility chart is a chart describing whether the ionic compounds formed from different combinations of cations and anions dissolve in or precipitate from solution.

Chart

The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate. For compounds with multiple hydrates, the solubility of the most soluble hydrate is shown.

Some compounds, such as nickel oxalate, will not precipitate immediately even though they are insoluble, requiring a few minutes to precipitate out.^[1]

Key
S	highly soluble or miscible	≥20 g/L
sS	slightly soluble	0.1~20 g/L
I	relatively insoluble	<0.1 g/L
R	reacts with or in water	N/a
?	unavailable	N/a

More information Ions names and symbols, Halogens ...

Ions names and symbols	Halogens					Chalcogens				Pnictogens		Crystallogens
Ions names and symbols	Fluoride F⁻	Chloride Cl⁻	Bromide Br⁻	Iodide I⁻	Perchlorate ClO⁻ ₄	Oxide O²⁻	Hydroxide OH⁻	Sulfide S²⁻	Sulfate SO²⁻ ₄	Nitrate NO⁻ ₃^[a]	Phosphate PO³⁻ ₄	Carbonate CO²⁻ ₃^[a]	Cyanide CN⁻	Thiocyanate SCN⁻	Acetate C ₂H ₃O⁻ ₂	Oxalate C ₂O²⁻ ₄
Hydrogen H⁺	S	S	S	S	S	N/A	N/A	sS	S	S	S	S	S	S	S	S
Ammonium NH⁺ ₄^[a]	S	S	S	S	S	S^[b]	S	R	S	S	S	S	S	S	S	S
Lithium Li⁺	sS	S	S	S	S	R	S	R	S	S	sS	sS	S	S	S	S
Sodium Na⁺	S	S	S	S	S	R	S	R	S	S	S	S	S	S	S	S
Potassium K⁺	S	S	S	S	sS	R	S	R	S	S	S	S	S	S	S	S
Rubidium Rb⁺	S	S	S	S	sS	R	S	R	S	S	S	S	S	S^[3]	S	S
Caesium Cs⁺	S	S	S	S	sS	R	S	R	S	S	S	S	S	S	S	S
Beryllium Be²⁺	S	S	S	R	S^[4]	I	I	R	S	S	I	sS	R	S^[5]	S	S
Magnesium Mg²⁺	sS	S	S	S	S	R	I	R	S	S	I	sS	R	S^[6]	S	sS
Calcium Ca²⁺	I	S	S	S	S	R	sS	R	sS	S	I	I	R	S^[7]	S	sS
Strontium Sr²⁺	sS	S	S	S	S	R	sS	R	sS	S	I	I	S	S^[8]	S	I
Barium Ba²⁺	sS	S	S	S	S	R	S	R	I	S	I^[9]	I	S	S	S	I
Aluminium Al³⁺	sS	S	S	S^[c]	S^[10]	I	I	R	S	S	I	R	R	S^[11]	S	I
Gallium Ga³⁺	I	S	S	R	S^[10]	I	I	R	sS	S	I	R	R	S^[12]	S	?
Manganese(II) Mn²⁺	sS	S	S	S	S^[13]	I	I	I	S	S	I	I	S	S^[14]	S	I
Iron(II) Fe²⁺	sS	S	S	S	S	I	I	I	S	S	I	I	?	S	S	sS
Cobalt(II) Co²⁺	sS	S	S	S	S^[15]	I	I	I	S	S	I	I	I	S	S	I
Nickel(II) Ni²⁺	S	S	S	S	S	I	I	I	S	S	I	I	I	S	S	I^[1]
Copper(II) Cu²⁺	sS	S	S	?	S	I	I	I	S	S	I	I^[d]	I	I	S	I
Zinc Zn²⁺	sS	S	S	S	S^[16]	I	I	I	S	S	I	I	I	S^[17]	S	I
Cadmium Cd²⁺	S	S	S	S	S^[18]	I	I	I	S	S	I	I	sS	sS^[17]	S	I
Mercury(II) Hg²⁺	R	S	sS	I	S^[19]	I	I	I	R	S	I	I	S	sS	S	sS^[20]
Vanadium(III) V³⁺	I	S	S	S	S^[21]	I	I	I	sS	S	I	?	?	S	?	?
Chromium(III) Cr³⁺	sS	S	S	S	S	I	I	I	S	S	I	I	S	S	S	?
Iron(III) Fe³⁺	S^[e]	S	S	R	S^[22]	I	I	I	S	S	sS	R^[23]	S	S^[24]	S^[25]^[f]	sS
Gold(III) Au³⁺	R	S	sS	?	?	I	I	I	?	?	I	I	S	?	sS	?
Tin(II) Sn²⁺	S	S	S	S	S^[26]	I	I	I	S	?	I	I	?	I^[27]	R	sS
Lead(II) Pb²⁺	sS	sS	sS	sS	S	I	sS	I	I	S	I	I	?^[28]	sS	S	I
Silver Ag⁺	S	I	I	I	S	I	I	I	sS	S	I	I	I	I	sS	I
Mercury(I) Hg²⁺ ₂	R	I	I	I	S^[29]	I	?	?	sS	S^[g]	?	I	I	?	S^[30]^[g]	?
	Fluoride F⁻	Chloride Cl⁻	Bromide Br⁻	Iodide I⁻	Perchlorate ClO⁻ ₄	Oxide O²⁻	Hydroxide OH⁻	Sulfide S²⁻	Sulfate SO²⁻ ₄	Nitrate NO⁻ ₃^[a]	Phosphate PO³⁻ ₄	Carbonate CO²⁻ ₃^[a]	Cyanide CN⁻	Thiocyanate SCN⁻	Acetate C ₂H ₃O⁻ ₂	Oxalate C ₂O²⁻ ₄

Notes

[a]
Compounds that include ammonium (NH⁺
₄), chlorate (ClO⁻
₃), or nitrate (NO⁻
₃) are soluble without exceptions. Compounds that include carbonate (CO²⁻
₃) are insoluble, unless the compound includes group 1 elements or ammonium.^[2]
[b]
"Ammonium oxide" does not exist. However, its theoretical molecular formula (NH⁺
₄)₂O²⁻ represents that of aqueous ammonia.
[c]
Partial electrolysis.
[d]
The commonly encountered basic copper carbonate (Cu₂CO₃(OH)₂) is insoluble in water. True copper(II) carbonate (CuCO₃) is rare and reacts with water to form basic copper carbonate.
[e]
Anhydrous FeF₃ is slightly soluble in water; FeF₃·3H₂O is much more soluble in water.
[f]
The commonly encountered basic iron(III) acetate ([Fe₃O(OAc)₆(H₂O)₃]OAc) is insoluble in water. True iron(III) acetate (Fe(OAc)₃) is rare and is soluble in water.
[g]
Slowly decomposes in water.

References

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Solubility chart

Chart

See also

Notes

References

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