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Solubility chart
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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
Shighly soluble or miscible≥20 g/L
sSslightly soluble0.1~20 g/L
Irelatively insoluble<0.1 g/L
Rreacts with or in water—
?unavailable—
Ions names and symbolsHalogensChalcogensPnictogensCrystallogens
FluorideF−ChlorideCl−BromideBr−IodideI−PerchlorateClO−4OxideO2−HydroxideOH−SulfideS2−SulfateSO2−4NitrateNO−32PhosphatePO3−4CarbonateCO2−33CyanideCN−ThiocyanateSCN−AcetateC2H3O−2OxalateC2O2−4
Hydrogen H+SSSSSSSsSSSSSSSSS
Ammonium NH+44SSSSSS5SRSSSSSSSS
Lithium Li+sSSSSSRSRSSsSsSSSSS
Sodium Na+SSSSSRSRSSSSSSSS
Potassium K+SSSSsSRSRSSSSSSSS
Rubidium Rb+SSSSsSRSRSSSSSS6SS
Caesium Cs+SSSSsSRSRSSSSSSSS
Beryllium Be2+SSSRS7IIRSSIsSRS8SS
Magnesium Mg2+sSSSSSRIRSSIsSRS9SsS
Calcium Ca2+ISSSSRsSRsSSIIRS10SsS
Strontium Sr2+sSSSSSRsSRsSSsSISS11SI
Barium Ba2+sSSSSSRSRISI12sSSSSI
Aluminium Al3+sSSSS13S14IIRSSIRRS15SI
Gallium Ga3+ISSRS16IIRsSSIRRS17S?
Manganese(II) Mn2+sSSSSS18IIISSIISS19SI
Iron(II) Fe2+sSSSSSIIISSIISSSsS
Cobalt(II) Co2+sSSSSS20IIISSIIISSI
Nickel(II) Ni2+SSSSSIIISSIIISSI21
Copper(II) Cu2+sSSS?SIIISSII22IISI
Zinc Zn2+sSSSSS23IIISSIIIS24SI
Cadmium Cd2+SSSSS25IIISSIIsSsS26SI
Mercury(II) Hg2+RSsSIS27IIIRSIISsSSsS28
Vanadium(III) V3+ISSSS29IIIsSSI??S??
Chromium(III) Cr3+sSSSSSIIISSIISSS?
Iron(III) Fe3+S30SSRS31IIISSsSR32SS33S3435sS
Gold(III) Au3+RSsS??III??IIS?sS?
Tin(II) Sn2+SSSSS36IIIS?II?I37RsS
Lead(II) Pb2+sSsSsSsSSIsSIISIIsSsSSI
Silver Ag+SIIISIIIsSSIIIIsSI
Mercury(I) Hg2+2RIIIS38I??sSS39?II?S4041?
 FluorideF−ChlorideCl−BromideBr−IodideI−PerchlorateClO−4OxideO2−HydroxideOH−SulfideS2−SulfateSO2−4NitrateNO−342PhosphatePO3−4CarbonateCO2−343CyanideCN−ThiocyanateSCN−AcetateC2H3O−2OxalateC2O2−4

See also

Notes

References

  1. J. A. Allen (1953). "The Precipitation of Nickel Oxalate". J. Phys. Chem. 57 (7): 715–716. doi:10.1021/j150508a027. /wiki/Doi_(identifier) ↩

  2. 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] /wiki/Alkali_metal ↩

  3. 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] /wiki/Alkali_metal ↩

  4. 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] /wiki/Alkali_metal ↩

  5. "Ammonium oxide" does not exist. However, its theoretical molecular formula (NH+4)2O2− represents that of aqueous ammonia. /wiki/Ammonia_solution ↩

  6. M. J. Joyce; F. Ninio (1989). "Raman Spectrum of Rubidium Thiocyanate at 37 K and Room Temperature". Australian Journal of Physics. 42 (4): 389–400. doi:10.1071/PH890389. https://doi.org/10.1071%2FPH890389 ↩

  7. 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. https://doi.org/10.3891%2Facta.chem.scand.15-1875 ↩

  8. W. J. Biermann; R. H. McCorkell (1967). "Liquid–liquid extraction of beryllium thiocyanate". Canadian Journal of Chemistry. 45 (22): 2846–2849. doi:10.1139/v67-459. https://doi.org/10.1139%2Fv67-459 ↩

  9. K. Mereiter; A. Preisinger (1982). "Structure of magnesium isothiocyanate tetrahydrate". Acta Crystallographica B. 38 (4): 1263–1265. doi:10.1107/S0567740882005433. /wiki/Doi_(identifier) ↩

  10. Claudia Wickleder; Patrick Larsen (2002). "Ca(SCN)2 and Ca(SCN)2 · 2 H2O: Crystal Structure, Thermal Behavior and Vibrational Spectroscopy". Zeitschrift für Naturforschung B. 57 (12): 1419–1426. doi:10.1515/znb-2002-1213. /wiki/Doi_(identifier) ↩

  11. Claudia Wickleder (2001). "M(SCN)2 (M = Eu, Sr, Ba): Kristallstruktur, thermisches Verhalten, Schwingungsspektroskopie". Zeitschrift für anorganische und allgemeine Chemie (in German). 627 (7): 1693–1698. doi:10.1002/1521-3749(200107)627:7<1693::AID-ZAAC1693>3.0.CO;2-U. /wiki/Doi_(identifier) ↩

  12. 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. Bibcode:2014JChEd..91.1261H. doi:10.1021/ed400741k. /wiki/Bibcode_(identifier) ↩

  13. Partial electrolysis. ↩

  14. 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. /wiki/Doi_(identifier) ↩

  15. S.J. Patel (1971). "Aluminium(III) isothiocyanate and its addition compounds". Journal of Inorganic and Nuclear Chemistry. 33 (1): 17–22. doi:10.1016/0022-1902(71)80004-0. /wiki/Doi_(identifier) ↩

  16. 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. /wiki/Doi_(identifier) ↩

  17. S. J. Patel; D. G. Tuck (1969). "Gallium(III) isothiocyanate and its addition compounds". Canadian Journal of Chemistry. 47 (2): 229–233. doi:10.1139/v69-032. /wiki/Doi_(identifier) ↩

  18. "44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis)". Alfa Aesar. Retrieved 16 September 2022. https://www.alfa.com/en/catalog/044318/ ↩

  19. B. Beagley; C.A. McAuliffe; A.G. Mackie; R.G. Pritchard (1984). "Preparation and crystal structure of manganese(II) isothiocyanate tetrahydrate". Inorganica Chimica Acta. 89 (3): 163–166. doi:10.1016/S0020-1693(00)82345-2. /wiki/Doi_(identifier) ↩

  20. E. Kamieńska-Piotrowicz (1999). "Conductometric Studies of Cobalt(II) Perchlorate in Acetonitrile-Water Solutions". Zeitschrift für Physikalische Chemie. 210 (1): 1–13. doi:10.1524/zpch.1999.210.Part_1.001. S2CID 102316324. /wiki/Doi_(identifier) ↩

  21. J. A. Allen (1953). "The Precipitation of Nickel Oxalate". J. Phys. Chem. 57 (7): 715–716. doi:10.1021/j150508a027. /wiki/Doi_(identifier) ↩

  22. 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. /wiki/Basic_copper_carbonate ↩

  23. Lili Lin; Xiaohua Liu; Xiaoming Feng (2014). "Zinc(II) Perchlorate Hexahydrate". Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons, Ltd: 1–5. doi:10.1002/047084289X.rn01657. ISBN 9780470842898. 9780470842898 ↩

  24. Masaki Kosaku (1931). "The Solubilities of Thiocyanate of Metals". Bulletin of the Chemical Society of Japan. 6 (7): 163–165. doi:10.1246/bcsj.6.163. https://doi.org/10.1246%2Fbcsj.6.163 ↩

  25. P. J. Reilly; R. H. Strokes (1971). "The diffusion coefficients of cadmium chloride and cadmium perchlorate in water at 25°". Australian Journal of Chemistry. 24 (7): 1361–1367. doi:10.1071/CH9711361. /wiki/Doi_(identifier) ↩

  26. Masaki Kosaku (1931). "The Solubilities of Thiocyanate of Metals". Bulletin of the Chemical Society of Japan. 6 (7): 163–165. doi:10.1246/bcsj.6.163. https://doi.org/10.1246%2Fbcsj.6.163 ↩

  27. 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. /wiki/Doi_(identifier) ↩

  28. "Properties of substance: mercury(II) oxalate Group of substances". Chemister. Retrieved 13 September 2022. http://chemister.ru/Database/properties-en.php?dbid=1&id=2631 ↩

  29. Burkhart, M J; Newton, T W (1969). "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. /wiki/Doi_(identifier) ↩

  30. Anhydrous FeF3 is slightly soluble in water; FeF3·3H2O is much more soluble in water. ↩

  31. M. Magini (1978). "An X-ray investigation on the structure of iron(III) perchlorate solutions". Journal of Inorganic and Nuclear Chemistry. 40 (1): 43–48. doi:10.1016/0022-1902(78)80304-2. /wiki/Doi_(identifier) ↩

  32. "Iron (III) Carbonate Formula". softschools.com. p. 1. Retrieved 19 August 2022. https://www.softschools.com/formulas/chemistry/iron_iii_carbonate_formula/670/#:~:text=Iron%20(III)%20carbonate%2C%20also,is%20291.72%20g%20mol%2D1. ↩

  33. Sano Hirotoshi; Akane Michiko (1973). "MÖSSBAUER SPECTROSCOPIC STUDIES ON IRON THIOCYANATE". Chemistry Letters. 2 (1): 43–46. doi:10.1246/cl.1973.43. /wiki/Doi_(identifier) ↩

  34. Ram C. Paul; Ramesh C. Narula; Sham K. Vasisht (1978). "Iron(III) acetates". Transition Metal Chemistry. 3: 35–38. doi:10.1007/BF01393501. S2CID 94447648. /wiki/Doi_(identifier) ↩

  35. 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. /wiki/Iron(III)_acetate ↩

  36. 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. /wiki/Doi_(identifier) ↩

  37. 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. /wiki/Doi_(identifier) ↩

  38. D. R. Rossėinsky (1963). "The reaction between mercury(I) and manganese(III) in aqueous perchlorate solution". Journal of the Chemical Society (Resumed): 1181–1186. doi:10.1039/JR9630001181. /wiki/Doi_(identifier) ↩

  39. Slowly decomposes in water. ↩

  40. National Center for Biotechnology Information. "PubChem Compound Summary for CID 61181, Mercurous acetate". PubChem. https://pubchem.ncbi.nlm.nih.gov/compound/Mercurous-acetate ↩

  41. Slowly decomposes in water. ↩

  42. 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] /wiki/Alkali_metal ↩

  43. 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] /wiki/Alkali_metal ↩