Solubility chart

For detailed information on exact solubility of compounds, see solubility table.

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	—
?	unavailable	—

Ions names and symbols	Halogens					Chalcogens				Pnictogens		Crystallogens
	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	sS	I	S	S[8]	S	I
Barium Ba2+	sS	S	S	S	S	R	S	R	I	S	I[9]	sS	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	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	sS	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[28]	I	?	?	sS	S[g]	?	I	I	?	S[29][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

See also

• Solubility rules

Notes

1. 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]
2. "Ammonium oxide" does not exist. However, its theoretical molecular formula (NH⁺
   ₄)₂O²⁻ represents that of aqueous ammonia.
3. Partial electrolysis.
4. 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.
5. Anhydrous FeF₃ is slightly soluble in water; FeF₃·3H₂O is much more soluble in water.
6. 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.
7. Slowly decomposes in water.