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Solubility chart

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

The following chart shows the solubility of various common ionic compounds in water, at a pressure of 1 atm and under room temperature (approx. 25 °C (298.15 K)). Boxes that read "soluble" indicate the formation of an aqueous product containing no precipitate, while "slightly soluble" and "insoluble" markings mean that a solid precipitate will form; "slightly soluble" compounds such as calcium sulfate may require heat to form precipitates. Boxes marked "other" can signify that many different states of products can result. For more detailed information on the exact solubility of compounds, see the solubility table.

For compounds with multiple hydrates, the solubility of the most soluble hydrate is shown in this chart.

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

Ions names and symbols Fluoride
F− 		Chloride
Cl− 		Bromide
Br− 		Iodide
I− 		Oxide
O2− 		Sulfide
S2− 		Hydroxide
OH− 		Cyanide
CN− 		Thiocyanate
SCN− 		Perchlorate
ClO−
4 		Nitrate
NO−
3[a] 		Acetate
C
2H
3O−
2 		Carbonate
CO2−
3[a] 		Sulfate
SO2−
4 		Oxalate
C
2O2−
4 		Phosphate
PO3−
4
Ammonium NH+
4[a] 		S S S S S* R S S S S S S S S S S
Hydrogen H+ S S S S S sS S S S S S S S S S S
Lithium Li+ sS S S S R R S S S S S S sS S S sS
Sodium Na+ S S S S R R S S S S S S S S S S
Potassium K+ S S S S R R S S S sS S S S S S S
Rubidium Rb+ S S S S R R S S S sS S S S S I S
Caesium Cs+ S S S S R R S S S sS S S S S I S
Beryllium Be2+ S S S R I R I R S S[3] S S sS S I S
Magnesium Mg2+ sS S S S I R I R S S S S sS S sS I
Calcium Ca2+ I S S S R R sS R S S S S I sS sS I
Strontium Sr2+ sS S S S R R sS S S S S S I sS I sS
Barium Ba2+ sS S S S R R S S S S S S sS I I I[4]
Aluminium Al3+ sS S S S[b] I R I R S S[5] S S R S I I
Gallium Ga3+ I S S R I R I ? S S[5] S S R sS ? I
Silver Ag+ S I I I I I I I I S S sS I sS I I
Mercury(I) Hg2+
2 		R I I I I ? ? I ? S S[c] S[6][c] I I ? ?
Thallium(I) Tl+ S sS sS I R I S S I[7] S S S S S sS sS
Manganese(II) Mn2+ sS S S S I I I S I S[8] S S I S I I
Iron(II) Fe2+ sS S S S I I I S S S S S I S sS I
Cobalt(II) Co2+ sS S S S I I I I S S[9] S S I S I I
Nickel(II) Ni2+ S S S S I I I I S S S S I S I[1] I
Copper(II) Cu2+ sS S S ? I I I I I S S S R[d] S I I
Zinc Zn2+ sS S S S I I I I S S[10] S S I S I I
Tin(II) Sn2+ S S S S I I I ? I[11] S[12] S R I S sS I
Mercury(II) Hg2+ R S S I I I I S sS S[13] S S I R sS[14] I
Lead(II) Pb2+ sS sS sS sS I I sS sS sS S S S I I I I
Vanadium(III) V3+ I S S S I I ? ? S S[15] S ? ? sS ? I
Chromium(III) Cr3+ sS S sS S I I I S S S S S I S ? I
Iron(III) Fe3+ S[e] S S R I I I S S S S I R[16] S sS sS
Gold Au3+ I S sS I I I I S ? ? S S I S ? ?
  Fluoride
F− 		Chloride
Cl− 		Bromide
Br− 		Iodide
I− 		Oxide
O2− 		Sulfide
S2− 		Hydroxide
OH− 		Cyanide
CN− 		Thiocyanate
SCN− 		Perchlorate
ClO−
4 		Nitrate
NO−
3[a] 		Acetate
C
2H
3O−
2 		Carbonate
CO2−
3[a] 		Sulfate
SO2−
4 		Oxalate
C
2O2−
4 		Phosphate
PO3−
4
  • Note: "Ammonium oxide" does not exist. However, its theoretical molecular formula (NH+
    4    )2O2− accurately represents that of aqueous ammonia.
Key (water needed to dissolve 1 gram of solute):
S soluble 0.01 ~ 50 mL
sS slightly soluble 50 mL ~ 10 L
I insoluble 10 L and up
X other —
R reacts with water —
? unavailable —

See also

Notes

  1. ^ a b c d e 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. ^ Partial electrolysis.
  3. ^ a b Slowly decomposes in water.
  4. ^ The commonly encountered basic copper carbonate (CuCO3(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.

References

  1. ^ a b J. A. Allen (1953). "The Precipitation of Nickel Oxalate". J. Phys. Chem. 57 (7): 715–716. doi:10.1021/j150508a027.
  2. ^ "Solubility Table". intro.chem.okstate.edu.
  3. ^ Birgitta Carell; Åke Olin (1961). "Studies on the Hydrolysis of Metal Ions. 37. Application of the Self-Medium Method to the Hydrolysis of Beryllium Perchlorate". Acta Chemica Scandinavica. 15: 1875–1884. doi:10.3891/acta.chem.scand.15-1875.
  4. ^ 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.
  5. ^ a b Laurence S. Foster (1939). "(I) The Reaction of Gallium with Perchloric Acid and (II) the Preparation and Properties of Gallium Perchlorate Hydrates". Journal of the American Chemical Society. 61 (11): 3122–3124. doi:10.1021/ja01266a041.
  6. ^ National Center for Biotechnology Information. "PubChem Compound Summary for CID 61181, Mercurous acetate". PubChem.
  7. ^ Popiel, Wojciech J.; Tamimi, Eid H. (1 July 1975). "Solubility product of thallium(I) thiocyanate in water at 10-40.deg". J. Chem. Eng. Data. 20 (3): 246–247. doi:10.1021/je60066a013.
  8. ^ "44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis)". Alfa Aesar. Alfa Aesar. Retrieved 16 September 2022.
  9. ^ E. Kamieńska-Piotrowicz (1999). "Conductometric Studies of Cobalt(II) Perchlorate in Acetonitrile-Water Solutions". Zeitschrift für Physikalische Chemie. 210 (1). doi:10.1524/zpch.1999.210.Part_1.001.
  10. ^ Lili Lin; Xiaohua Liu; Xiaoming Feng (2014). "Zinc(II) Perchlorate Hexahydrate". Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons, Ltd. doi:10.1002/047084289X.rn01657.
  11. ^ Tewfik B. Absi; Ramesh C. Makhija; Mario Onyszchuk (1978). "Synthesis and vibrational spectra of tin(II) isothiocyanate adducts with some O- and N-donor ligands". Canadian Journal of Chemistry. 56 (15): 2039–2041. doi:10.1139/v78-333.
  12. ^ C.G.Davies; J.D.Donaldson (1968). "Tin(II) perchlorate trihydrate". Journal of Inorganic and Nuclear Chemistry. 30 (10). Chelsea College of Science and Technology: 2635–2639. doi:10.1016/0022-1902(68)80389-6.
  13. ^ Franco Cristiani; Francesco Demartin; Francesco A. Devillanova; Angelo Diaz; Francesco Isaia; Gaetano Verani (1990). "Reactivity of Mercury(II) Perchlorate Towards 5,5 -Dimethylimidazolidine-2- Thione-4-One. Structure of Bis(5,5-Dimethylimidazolidine-2-Thione-4-One)Mercury(II) Perchlorate Triaquo". Journal of Coordination Chemistry. 21 (2): 137–146. doi:10.1080/00958979009409182.
  14. ^ "Properties of substance: mercury(II) oxalate Group of substances:". Chemister. Chemister. Retrieved 13 September 2022.
  15. ^ Burkhart, M J; Newton, T W (1969). "THE KINETICS OF THE REACTION BETWEEN VANADIUM(II) AND NEPTUNIUM(IV) IN AQUEOUS PERCHLORATE SOLUTIONS". J. Phys. Chem. 73 (6): 1741–1746. doi:10.1021/j100726a018.
  16. ^ "Iron (III) Carbonate Formula". softschools.com. p. 1. Retrieved 19 August 2022.
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