The following chart shows thesolubility 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 likecalcium sulfate may require heat to precipitate. For compounds with multiple hydrates, the solubility of the most soluble hydrate is shown.
Some compounds, such asnickel oxalate, will not precipitate immediately even though they are insoluble, requiring a few minutes to precipitate out.[1]
^abcdeCompounds 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 includesgroup 1 elements or ammonium.[2]
^"Ammonium oxide" does not exist. However, its theoretical molecular formula (NH+ 4)2O2− represents that ofaqueous ammonia.
^The commonly encounteredbasic copper carbonate (Cu2CO3(OH)2) is insoluble in water. Truecopper(II) carbonate (CuCO3) is rare and reacts with water to form basic copper carbonate.
^Anhydrous FeF3 is slightly soluble in water; FeF3·3H2O is much more soluble in water.
^The commonly encounteredbasic 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.
^K. Mereiter; A. Preisinger (1982). "Structure of magnesium isothiocyanate tetrahydrate".Acta Crystallographica B.38 (4):1263–1265.doi:10.1107/S0567740882005433.
^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.
^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.
^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.
^abLaurence 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.
^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.
^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.
^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.
^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.S2CID102316324.
^Lili Lin; Xiaohua Liu; Xiaoming Feng (2014). "Zinc(II) Perchlorate Hexahydrate".Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons, Ltd. pp. 1–5.doi:10.1002/047084289X.rn01657.ISBN9780470842898.
^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.
^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.
^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.
^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.
^Sano Hirotoshi; Akane Michiko (1973). "MÖSSBAUER SPECTROSCOPIC STUDIES ON IRON THIOCYANATE".Chemistry Letters.2 (1):43–46.doi:10.1246/cl.1973.43.
^Ram C. Paul; Ramesh C. Narula; Sham K. Vasisht (1978). "Iron(III) acetates".Transition Metal Chemistry.3:35–38.doi:10.1007/BF01393501.S2CID94447648.
^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.
^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.
^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.
