Solubility chart explained

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.). "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

	Halogens					Chalcogens				Pnictogens		Crystallogens
	Fluoride F^−	Chloride Cl^−	Bromide Br^−	Iodide I^−	Perchlorate	Oxide O^2−	Hydroxide OH^−	Sulfide S^2−	Sulfate	Nitrate	Phosphate	Carbonate	Cyanide CN^−	Thiocyanate SCN^−	Acetate	Oxalate
Hydrogen H^+	S	S	S	S	S	S	S	sS	S	S	S	S	S	S	S	S
	S	S	S	S	S	S	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^[2]	S	S
Caesium Cs^+	S	S	S	S	sS	R	S	R	S	S	S	S	S	S	S	S
Beryllium Be^2+	S	S	S	R	S^[3]	I	I	R	S	S	I	sS	R	S^[4]	S	S
Magnesium Mg^2+	sS	S	S	S	S	R	I	R	S	S	I	sS	R	S^[5]	S	sS
Calcium Ca^2+	I	S	S	S	S	R	sS	R	sS	S	I	I	R	S^[6]	S	sS
Strontium Sr^2+	sS	S	S	S	S	R	sS	R	sS	S	sS	I	S	S^[7]	S	I
Barium Ba^2+	sS	S	S	S	S	R	S	R	I	S	I^[8]	sS	S	S	S	I
Aluminium Al^3+	sS	S	S	S	S	I	I	R	S	S	I	R	R	S^[9]	S	I
Gallium Ga^3+	I	S	S	R	S^[10]	I	I	R	sS	S	I	R	R	S^[11]	S	?
Manganese(II) Mn^2+	sS	S	S	S	S^[12]	I	I	I	S	S	I	I	S	S^[13]	S	I
Iron(II) Fe^2+	sS	S	S	S	S	I	I	I	S	S	I	I	S	S	S	sS
Cobalt(II) Co^2+	sS	S	S	S	S^[14]	I	I	I	S	S	I	I	I	S	S	I
Nickel(II) Ni^2+	S	S	S	S	S	I	I	I	S	S	I	I	I	S	S	I
Copper(II) Cu^2+	sS	S	S	?	S	I	I	I	S	S	I	I	I	I	S	I
Zinc Zn^2+	sS	S	S	S	S^[15]	I	I	I	S	S	I	I	I	S^[16]	S	I
Cadmium Cd^2+	S	S	S	S	S^[17]	I	I	I	S	S	I	I	sS	sS	S	I
Mercury(II) Hg^2+	R	S	sS	I	S^[18]	I	I	I	R	S	I	I	S	sS	S	sS^[19]
Vanadium(III) V^3+	I	S	S	S	S^[20]	I	I	I	sS	S	I	?	?	S	?	?
Chromium(III) Cr^3+	sS	S	S	S	S	I	I	I	S	S	I	I	S	S	S	?
Iron(III) Fe^3+	S	S	S	R	S^[21]	I	I	I	S	S	sS	R^[22]	S	S^[23]	S^[24]	sS
Gold(III) Au^3+	R	S	sS	?	?	I	I	I	?	?	I	I	S	?	sS	?
Tin(II) Sn^2+	S	S	S	S	S^[25]	I	I	I	S	?	I	I	?	I^[26]	R	sS
Lead(II) Pb^2+	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)	R	I	I	I	S^[27]	I	?	?	sS	S	?	I	I	?	S^[28]	?
	Fluoride F^−	Chloride Cl^−	Bromide Br^−	Iodide I^−	Perchlorate	Oxide O^2−	Hydroxide OH^−	Sulfide S^2−	Sulfate	Nitrate	Phosphate	Carbonate	Cyanide CN^−	Thiocyanate SCN^−	Acetate	Oxalate

See also

• Solubility rules

Notes and References

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3. Birgitta Carell . Åke Olin . Studies on the Hydrolysis of Metal Ions. 37. Application of the Self-Medium Method to the Hydrolysis of Beryllium Perchlorate. . Acta Chemica Scandinavica . 1961 . 15 . 1875–1884 . 10.3891/acta.chem.scand.15-1875 . English. free .
4. W. J. Biermann . R. H. McCorkell . Liquid–liquid extraction of beryllium thiocyanate . Canadian Journal of Chemistry . 1967 . 45 . 22 . 2846-2849 . 10.1139/v67-459 . en. free .
5. K. Mereiter . A. Preisinger . Structure of magnesium isothiocyanate tetrahydrate . Acta Crystallographica B . 1982 . 38 . 1263-1265 . 10.1107/S0567740882005433 . en.
6. Claudia Wickleder . Patrick Larsen . Ca(SCN)2 and Ca(SCN)2 · 2 H2O: Crystal Structure, Thermal Behavior and Vibrational Spectroscopy . Zeitschrift für Naturforschung B . 2002 . 57 . 12 . 1419–1426 . 10.1515/znb-2002-1213 . en.
7. Claudia Wickleder . M(SCN)2 (M = Eu, Sr, Ba): Kristallstruktur, thermisches Verhalten, Schwingungsspektroskopie . Zeitschrift für anorganische und allgemeine Chemie . 2001 . 627 . 7 . 1693-1698 . 10.1002/1521-3749(200107)627:7<1693::AID-ZAAC1693>3.0.CO;2-U . de.
8. 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. Hazen . Jeffery L. . Cleary . David A. . July 2, 2014 . 10.1021/ed400741k . 2014JChEd..91.1261H .
9. S.J. Patel . Aluminium(III) isothiocyanate and its addition compounds . Journal of Inorganic and Nuclear Chemistry . 1971 . 33 . 1 . 17-22 . 10.1016/0022-1902(71)80004-0 . en.
10. Laurence S. Foster . (I) The Reaction of Gallium with Perchloric Acid and (II) the Preparation and Properties of Gallium Perchlorate Hydrates . Journal of the American Chemical Society . 1939 . 61 . 11 . 3122–3124 . 10.1021/ja01266a041 . English.
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12. Web site: 44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis) . Alfa Aesar . Alfa Aesar . 16 September 2022.
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14. E. Kamieńska-Piotrowicz . Conductometric Studies of Cobalt(II) Perchlorate in Acetonitrile-Water Solutions . Zeitschrift für Physikalische Chemie . 1999 . 210 . 1 . 1–13 . 10.1524/zpch.1999.210.Part_1.001 . 102316324 . en.
15. Lili Lin . Xiaohua Liu . Xiaoming Feng . Zinc(II) Perchlorate Hexahydrate . Encyclopedia of Reagents for Organic Synthesis . 2014 . 1–5 . 10.1002/047084289X.rn01657 . John Wiley & Sons, Ltd . 9780470842898 . en.
16. Masaki Kosaku . THE SOLUBILITIES OF THIOCYANATE OF METALS . Bulletin of the Chemical Society of Japan . 1931 . 6 . 7 . 163-165 . 10.1246/bcsj.6.163 . en. free .
17. P. J. Reilly . R. H. Strokes . The diffusion coefficients of cadmium chloride and cadmium perchlorate in water at 25° . Australian Journal of Chemistry . 1971 . 24 . 7 . 1361-1367 . 10.1071/CH9711361 . en.
18. Franco Cristiani . Francesco Demartin . Francesco A. Devillanova . Angelo Diaz . Francesco Isaia . Gaetano Verani . 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 . 1990 . 21 . 2 . 137–146 . 10.1080/00958979009409182 . en.
19. Web site: Properties of substance: mercury(II) oxalate Group of substances . Chemister . Chemister . 13 September 2022 . English.
20. Burkhart, M J . Newton, T W . Kinetics of the reaction between vanadium(II) and neptunium(IV) in aqueous perchlorate solutions . J. Phys. Chem. . 1969 . 73 . 6 . 1741–1746 . 10.1021/j100726a018 . en.
21. M. Magini . An X-ray investigation on the structure of iron(III) perchlorate solutions . Journal of Inorganic and Nuclear Chemistry . 1978 . 40 . 1 . 43-48 . 10.1016/0022-1902(78)80304-2 . en.
22. Web site: Iron (III) Carbonate Formula . softschools.com . 19 August 2022 . 1.
23. Sano Hirotoshi . Akane Michiko . MÖSSBAUER SPECTROSCOPIC STUDIES ON IRON THIOCYANATE . Chemistry Letters . 1973 . 2 . 1 . 43-46 . 10.1246/cl.1973.43 . en.
24. Ram C. Paul . Ramesh C. Narula . Sham K. Vasisht . Iron(III) acetates . Transition Metal Chemistry . 1978 . 3 . 35–38 . 10.1007/BF01393501 . 94447648 . en.
25. C.G.Davies . J.D.Donaldson . Tin(II) perchlorate trihydrate . Journal of Inorganic and Nuclear Chemistry . 1968 . 30 . 10 . 2635–2639 . 10.1016/0022-1902(68)80389-6 . Chelsea College of Science and Technology . en.
26. Tewfik B. Absi . Ramesh C. Makhija . Mario Onyszchuk . Synthesis and vibrational spectra of tin(II) isothiocyanate adducts with some O- and N-donor ligands . Canadian Journal of Chemistry . 1978 . 56 . 15 . 2039–2041 . 10.1139/v78-333 . English.
27. D. R. Rossėinsky . The reaction between mercury(I) and manganese(III) in aqueous perchlorate solution . Journal of the Chemical Society (Resumed) . 1963 . 1181-1186 . 10.1039/JR9630001181 . en.
28. Web site: National Center for Biotechnology Information . PubChem Compound Summary for CID 61181, Mercurous acetate . PubChem.