Solubility chart

{{Short description|Chart describing whether ionic compounds dissolve or precipitate}}

{{For|detailed information on exact solubility of compounds|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. {{cvt|25|C|K|2|disp=comma}}). "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.{{cite journal |author1=J. A. Allen |title=The Precipitation of Nickel Oxalate |journal=J. Phys. Chem. |date=1953 |volume=57 |issue=7 |pages=715–716 |doi=10.1021/j150508a027 |language=en}}

class="wikitable" \|+ Key
bgcolor="#99CCFF" align="center" \| S	highly soluble or miscible	≥20 g/L
bgcolor="#CCCCFF" align="center" \| sS	slightly soluble	0.1~20 g/L
bgcolor="#FFCCCC" align="center" \| I	relatively insoluble	<0.1 g/L
bgcolor="#CCCCCC" align="center" \| R	reacts with or in water	{{N/A}}
align="center" \| ?	unavailable	{{N/A}}

class="wikitable" style="font-size:85%" ! rowspan="2" \|{{Nowrap\|Ions names and symbols}} ! colspan="5" \|Halogens ! colspan="4" \|Chalcogens ! colspan="2" \|Pnictogens ! colspan="5" \|Crystallogens
Fluoride F⁻ ! Chloride Cl⁻ ! Bromide Br⁻ ! Iodide I⁻ ! Perchlorate {{chem\|ClO\|4\|−}} ! Oxide O²⁻ ! Hydroxide OH⁻ ! Sulfide S²⁻ ! Sulfate {{chem\|SO\|4\|2−}} ! Nitrate {{chem\|NO\|3\|−}}{{efn\|name=AlwaysSolubleK\|group=lower-alpha\|Compounds that include ammonium ({{chem\|NH\|4\|+}}), chlorate ({{chem\|ClO\|3\|−}}), or nitrate ({{chem\|NO\|3\|−}}) are soluble without exceptions. Compounds that include carbonate ({{chem\|CO\|3\|2−}}) are insoluble, unless the compound includes group 1 elements or ammonium.{{cite web \|url=http://intro.chem.okstate.edu/1515SP01/Database/Solub.html \|title=Solubility Table \|website=intro.chem.okstate.edu}}}} ! Phosphate {{chem\|PO\|4\|3−}} ! Carbonate {{chem\|CO\|3\|2−}}{{efn\|name=AlwaysSolubleK}} ! Cyanide CN⁻ ! Thiocyanate SCN⁻ ! Acetate {{chem\|C\|2\|H\|3\|O\|2\|−}} ! Oxalate {{chem\|C\|2\|O\|4\|2−}}
align="center" ! Hydrogen H⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Ammonium {{chem\|NH\|4\|+}}{{efn\|name=AlwaysSolubleK}} \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{efn\|group=lower-alpha\|"Ammonium oxide" does not exist. However, its theoretical molecular formula ({{chem\|NH\|4\|+}})₂O²⁻ represents that of aqueous ammonia.}} \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Lithium Li⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Sodium Na⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Potassium K⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Rubidium Rb⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=M. J. Joyce \|author2=F. Ninio \|title=Raman Spectrum of Rubidium Thiocyanate at 37 K and Room Temperature \|journal=Australian Journal of Physics \|date=1989 \|volume=42 \|issue=4 \|pages=389–400 \|doi=10.1071/PH890389 \|language=en\|doi-access=free }} \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Caesium Cs⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Beryllium Be²⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Birgitta Carell \|author2=Åke Olin \|title=Studies on the Hydrolysis of Metal Ions. 37. Application of the Self-Medium Method to the Hydrolysis of Beryllium Perchlorate. \|journal=Acta Chemica Scandinavica \|date=1961 \|volume=15 \|pages=1875–1884 \|doi=10.3891/acta.chem.scand.15-1875 \|language=English\|doi-access=free }} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=W. J. Biermann \|author2=R. H. McCorkell \|title=Liquid–liquid extraction of beryllium thiocyanate \|journal=Canadian Journal of Chemistry \|date=1967 \|volume=45 \|issue=22 \|pages=2846–2849 \|doi=10.1139/v67-459 \|language=en\|doi-access=free }} \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S
align="center" ! Magnesium Mg²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=K. Mereiter \|author2=A. Preisinger \|title=Structure of magnesium isothiocyanate tetrahydrate \|journal=Acta Crystallographica B \|date=1982 \|volume=38 \|issue=4 \|pages=1263–1265 \|doi=10.1107/S0567740882005433 \|language=en}} \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS
align="center" ! Calcium Ca²⁺ \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Claudia Wickleder \|author2=Patrick Larsen \|title=Ca(SCN)2 and Ca(SCN)2 · 2 H2O: Crystal Structure, Thermal Behavior and Vibrational Spectroscopy \|journal=Zeitschrift für Naturforschung B \|date=2002 \|volume=57 \|issue=12 \|pages=1419–1426 \|doi=10.1515/znb-2002-1213 \|language=en}} \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS
align="center" ! Strontium Sr²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Claudia Wickleder \|title=M(SCN)2 (M = Eu, Sr, Ba): Kristallstruktur, thermisches Verhalten, Schwingungsspektroskopie \|journal=Zeitschrift für anorganische und allgemeine Chemie \|date=2001 \|volume=627 \|issue=7 \|pages=1693–1698 \|doi=10.1002/1521-3749(200107)627:7<1693::AID-ZAAC1693>3.0.CO;2-U \|language=de}} \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Barium Ba²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I{{Cite journal \|title=Yielding Unexpected Results: Precipitation of Ba₃(PO₄)₂ and Implications for Teaching Solubility Principles in the General Chemistry Curriculum \|journal = Journal of Chemical Education\|volume = 91\|issue = 8\|pages = 1261–1263\|last1=Hazen \|first1=Jeffery L. \|last2=Cleary \|first2=David A. \|date=July 2, 2014 \|doi=10.1021/ed400741k \| bibcode=2014JChEd..91.1261H }} \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Aluminium Al³⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{efn\|Partial electrolysis.}} \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=S.J. Patel \|title=Aluminium(III) isothiocyanate and its addition compounds \|journal=Journal of Inorganic and Nuclear Chemistry \|date=1971 \|volume=33 \|issue=1 \|pages=17–22 \|doi=10.1016/0022-1902(71)80004-0 \|language=en}} \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Gallium Ga³⁺ \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Laurence S. Foster \|title=(I) The Reaction of Gallium with Perchloric Acid and (II) the Preparation and Properties of Gallium Perchlorate Hydrates \|journal=Journal of the American Chemical Society \|date=1939 \|volume=61 \|issue=11 \|pages=3122–3124 \|doi=10.1021/ja01266a041 \|language=English}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=S. J. Patel \|author2=D. G. Tuck \|title=Gallium(III) isothiocyanate and its addition compounds \|journal=Canadian Journal of Chemistry \|date=1969 \|volume=47 \|issue=2 \|pages=229–233 \|doi=10.1139/v69-032 \|language=en}} \| bgcolor="#99CCFF" \| S \| ?
align="center" ! Manganese(II) Mn²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite web \|title=44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis) \|url=https://www.alfa.com/en/catalog/044318/ \|website=Alfa Aesar \|access-date=16 September 2022}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=B. Beagley \|author2=C.A. McAuliffe \|author3=A.G. Mackie \|author4=R.G. Pritchard \|title=Preparation and crystal structure of manganese(II) isothiocyanate tetrahydrate \|journal=Inorganica Chimica Acta \|date=1984 \|volume=89 \|issue=3 \|pages=163–166 \|doi=10.1016/S0020-1693(00)82345-2 \|language=en}} \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Iron(II) Fe²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS
align="center" ! Cobalt(II) Co²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=E. Kamieńska-Piotrowicz \|title=Conductometric Studies of Cobalt(II) Perchlorate in Acetonitrile-Water Solutions \|journal=Zeitschrift für Physikalische Chemie \|date=1999 \|volume=210 \|issue=1 \|pages=1–13 \|doi=10.1524/zpch.1999.210.Part_1.001 \|s2cid=102316324 \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Nickel(II) Ni²⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Copper(II) Cu²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| ? \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I{{efn\|group=lower-alpha\|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.}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Zinc Zn²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Lili Lin \|author2=Xiaohua Liu \|author3=Xiaoming Feng \|title=Zinc(II) Perchlorate Hexahydrate \|journal=Encyclopedia of Reagents for Organic Synthesis \|date=2014 \|pages=1–5 \|doi=10.1002/047084289X.rn01657 \|publisher=John Wiley & Sons, Ltd \|isbn=9780470842898 \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Masaki Kosaku \|title=The Solubilities of Thiocyanate of Metals \|journal=Bulletin of the Chemical Society of Japan \|date=1931 \|volume=6 \|issue=7 \|pages=163–165 \|doi=10.1246/bcsj.6.163 \|language=en\|doi-access=free }} \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Cadmium Cd²⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=P. J. Reilly \|author2=R. H. Strokes \|title=The diffusion coefficients of cadmium chloride and cadmium perchlorate in water at 25° \|journal=Australian Journal of Chemistry \|date=1971 \|volume=24 \|issue=7 \|pages=1361–1367 \|doi=10.1071/CH9711361 \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Mercury(II) Hg²⁺ \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Franco Cristiani \|author2=Francesco Demartin \|author3=Francesco A. Devillanova \|author4=Angelo Diaz \|author5=Francesco Isaia \|author6=Gaetano Verani \|title=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=Journal of Coordination Chemistry \|date=1990 \|volume=21 \|issue=2 \|pages=137–146 \|doi=10.1080/00958979009409182 \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS{{cite web \|title=Properties of substance: mercury(II) oxalate Group of substances \|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=2631 \|website=Chemister \|access-date=13 September 2022 \|language=English}}
align="center" ! Vanadium(III) V³⁺ \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Burkhart, M J \|author2=Newton, T W \|title=Kinetics of the reaction between vanadium(II) and neptunium(IV) in aqueous perchlorate solutions \|journal=J. Phys. Chem. \|date=1969 \|volume=73 \|issue=6 \|pages=1741–1746 \|doi=10.1021/j100726a018 \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| ? \| ? \| bgcolor="#99CCFF" \| S \| ? \| ?
align="center" ! Chromium(III) Cr³⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| ?
align="center" ! Iron(III) Fe³⁺ \| bgcolor="#99CCFF" \| S{{efn\|group=lower-alpha\|Anhydrous FeF₃ is slightly soluble in water; FeF₃·3H₂O is much more soluble in water.}} \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S{{cite journal \|author1=M. Magini \|title=An X-ray investigation on the structure of iron(III) perchlorate solutions \|journal=Journal of Inorganic and Nuclear Chemistry \|date=1978 \|volume=40 \|issue=1 \|pages=43–48 \|doi=10.1016/0022-1902(78)80304-2 \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCCC" \| R{{Cite web \|title=Iron (III) Carbonate Formula \|website=softschools.com \|access-date=19 August 2022 \|pages = 1\|url=https://www.softschools.com/formulas/chemistry/iron_iii_carbonate_formula/670/#:~:text=Iron%20(III)%20carbonate%2C%20also,is%20291.72%20g%20mol%2D1.}} \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Sano Hirotoshi \|author2=Akane Michiko \|title=MÖSSBAUER SPECTROSCOPIC STUDIES ON IRON THIOCYANATE \|journal=Chemistry Letters \|date=1973 \|volume=2 \|issue=1 \|pages=43–46 \|doi=10.1246/cl.1973.43 \|language=en}} \| bgcolor="#99CCFF" \| S{{cite journal \|author1=Ram C. Paul \|author2=Ramesh C. Narula \|author3=Sham K. Vasisht \|title=Iron(III) acetates \|journal=Transition Metal Chemistry \|date=1978 \|volume=3 \|pages=35–38 \|doi=10.1007/BF01393501 \|s2cid=94447648 \|language=en}}{{efn\|group=lower-alpha\|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.}} \| bgcolor="#CCCCFF" \| sS
align="center" ! Gold(III) Au³⁺ \| bgcolor="#CCCCCC" \| R \| bgcolor="#99CCFF" \| S \| bgcolor="#CCCCFF" \| sS \| ? \| ? \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| ? \| ? \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| ? \| bgcolor="#CCCCFF" \| sS \| ?
align="center" ! Tin(II) Sn²⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S \| bgcolor="#99CCFF" \| S{{cite journal \|author1=C.G.Davies \|author2=J.D.Donaldson \|title=Tin(II) perchlorate trihydrate \|journal=Journal of Inorganic and Nuclear Chemistry \|date=1968 \|volume=30 \|issue=10 \|pages=2635–2639 \|doi=10.1016/0022-1902(68)80389-6 \|location=Chelsea College of Science and Technology \|language=en}} \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| ? \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| ? \| bgcolor="#FFCCCC" \| I{{cite journal \|author1=Tewfik B. Absi \|author2=Ramesh C. Makhija \|author3=Mario Onyszchuk \|title=Synthesis and vibrational spectra of tin(II) isothiocyanate adducts with some O- and N-donor ligands \|journal=Canadian Journal of Chemistry \|date=1978 \|volume=56 \|issue=15 \|pages=2039–2041 \|doi=10.1139/v78-333 \|language=English}} \| bgcolor="#CCCCCC" \| R \| bgcolor="#CCCCFF" \| sS
align="center" ! Lead(II) Pb²⁺ \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I
align="center" ! Silver Ag⁺ \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#CCCCFF" \| sS \| bgcolor="#FFCCCC" \| I
align="center" ! Mercury(I) {{chem\|Hg\|2\|2+}} \| bgcolor="#CCCCCC" \| R \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| bgcolor="#99CCFF" \| S{{cite journal \|author1=D. R. Rossėinsky \|title=The reaction between mercury(I) and manganese(III) in aqueous perchlorate solution \|journal=Journal of the Chemical Society (Resumed) \|date=1963 \|pages=1181–1186 \|doi=10.1039/JR9630001181 \|language=en}} \| bgcolor="#FFCCCC" \| I \| ? \| ? \| bgcolor="#CCCCFF" \| sS \| bgcolor="#99CCFF" \| S{{efn\|name=MercurousSlowReact\|group=lower-alpha\|Slowly decomposes in water.}} \| ? \| bgcolor="#FFCCCC" \| I \| bgcolor="#FFCCCC" \| I \| ? \| bgcolor="#99CCFF" \| S{{cite web \|last1=National Center for Biotechnology Information \|title=PubChem Compound Summary for CID 61181, Mercurous acetate \|url=https://pubchem.ncbi.nlm.nih.gov/compound/Mercurous-acetate \|website=PubChem}}{{efn\|name=MercurousSlowReact}} \| ?
width="5.88%" \| ! width="5.88%" \| Fluoride F⁻ ! width="5.88%" \| Chloride Cl⁻ ! width="5.88%" \| Bromide Br⁻ ! width="5.88%" \| Iodide I⁻ ! width="5.88%" \| Perchlorate {{chem\|ClO\|4\|−}} ! width="5.88%" \| Oxide O²⁻ ! width="5.88%" \| Hydroxide OH⁻ ! width="5.88%" \| Sulfide S²⁻ ! width="5.88%" \| Sulfate {{chem\|SO\|4\|2−}} ! width="5.88%" \| Nitrate {{chem\|NO\|3\|−}}{{efn\|name=AlwaysSolubleK}} ! width="5.88%" \| Phosphate {{chem\|PO\|4\|3−}} ! width="5.88%" \| Carbonate {{chem\|CO\|3\|2−}}{{efn\|name=AlwaysSolubleK}} ! width="5.88%" \| Cyanide CN⁻ ! width="5.88%" \| Thiocyanate SCN⁻ ! width="5.88%" \| Acetate {{chem\|C\|2\|H\|3\|O\|2\|−}} ! width="5.88%" \| Oxalate {{chem\|C\|2\|O\|4\|2−}}

class="wikitable" style="font-size:85%"

! rowspan="2" |{{Nowrap|Ions names and symbols}}

! colspan="5" |Halogens

! colspan="4" |Chalcogens

! colspan="2" |Pnictogens

! colspan="5" |Crystallogens

Fluoride
F⁻

! Chloride
Cl⁻

! Bromide
Br⁻

! Iodide
I⁻

! Perchlorate
{{chem|ClO|4|−}}

! Oxide
O²⁻

! Hydroxide
OH⁻

! Sulfide
S²⁻

! Sulfate
{{chem|SO|4|2−}}

! Nitrate
{{chem|NO|3|−}}{{efn|name=AlwaysSolubleK|group=lower-alpha|Compounds that include ammonium ({{chem|NH|4|+}}), chlorate ({{chem|ClO|3|−}}), or nitrate ({{chem|NO|3|−}}) are soluble without exceptions. Compounds that include carbonate ({{chem|CO|3|2−}}) are insoluble, unless the compound includes group 1 elements or ammonium.{{cite web |url=http://intro.chem.okstate.edu/1515SP01/Database/Solub.html |title=Solubility Table |website=intro.chem.okstate.edu}}}}

! Phosphate
{{chem|PO|4|3−}}

! Carbonate
{{chem|CO|3|2−}}{{efn|name=AlwaysSolubleK}}

! Cyanide
CN⁻

! Thiocyanate
SCN⁻

! Acetate
{{chem|C|2|H|3|O|2|−}}

! Oxalate
{{chem|C|2|O|4|2−}}

align="center"

! Hydrogen H⁺

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

align="center"

! Ammonium {{chem|NH|4|+}}{{efn|name=AlwaysSolubleK}}

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{efn|group=lower-alpha|"Ammonium oxide" does not exist. However, its theoretical molecular formula ({{chem|NH|4|+}})₂O²⁻ represents that of aqueous ammonia.}}

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

align="center"

! Lithium Li⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

align="center"

! Sodium Na⁺

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

align="center"

! Potassium K⁺

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

align="center"

! Rubidium Rb⁺

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=M. J. Joyce |author2=F. Ninio |title=Raman Spectrum of Rubidium Thiocyanate at 37 K and Room Temperature |journal=Australian Journal of Physics |date=1989 |volume=42 |issue=4 |pages=389–400 |doi=10.1071/PH890389 |language=en|doi-access=free }}

| bgcolor="#99CCFF" | S

align="center"

! Caesium Cs⁺

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

align="center"

! Beryllium Be²⁺

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=Birgitta Carell |author2=Åke Olin |title=Studies on the Hydrolysis of Metal Ions. 37. Application of the Self-Medium Method to the Hydrolysis of Beryllium Perchlorate. |journal=Acta Chemica Scandinavica |date=1961 |volume=15 |pages=1875–1884 |doi=10.3891/acta.chem.scand.15-1875 |language=English|doi-access=free }}

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=W. J. Biermann |author2=R. H. McCorkell |title=Liquid–liquid extraction of beryllium thiocyanate |journal=Canadian Journal of Chemistry |date=1967 |volume=45 |issue=22 |pages=2846–2849 |doi=10.1139/v67-459 |language=en|doi-access=free }}

| bgcolor="#99CCFF" | S

align="center"

! Magnesium Mg²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=K. Mereiter |author2=A. Preisinger |title=Structure of magnesium isothiocyanate tetrahydrate |journal=Acta Crystallographica B |date=1982 |volume=38 |issue=4 |pages=1263–1265 |doi=10.1107/S0567740882005433 |language=en}}

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

align="center"

! Calcium Ca²⁺

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=Claudia Wickleder |author2=Patrick Larsen |title=Ca(SCN)2 and Ca(SCN)2 · 2 H2O: Crystal Structure, Thermal Behavior and Vibrational Spectroscopy |journal=Zeitschrift für Naturforschung B |date=2002 |volume=57 |issue=12 |pages=1419–1426 |doi=10.1515/znb-2002-1213 |language=en}}

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

align="center"

! Strontium Sr²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=Claudia Wickleder |title=M(SCN)2 (M = Eu, Sr, Ba): Kristallstruktur, thermisches Verhalten, Schwingungsspektroskopie |journal=Zeitschrift für anorganische und allgemeine Chemie |date=2001 |volume=627 |issue=7 |pages=1693–1698 |doi=10.1002/1521-3749(200107)627:7<1693::AID-ZAAC1693>3.0.CO;2-U |language=de}}

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Barium Ba²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I{{Cite journal |title=Yielding Unexpected Results: Precipitation of Ba₃(PO₄)₂ and Implications for Teaching Solubility Principles in the General Chemistry Curriculum |journal = Journal of Chemical Education|volume = 91|issue = 8|pages = 1261–1263|last1=Hazen |first1=Jeffery L. |last2=Cleary |first2=David A. |date=July 2, 2014 |doi=10.1021/ed400741k | bibcode=2014JChEd..91.1261H }}

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Aluminium Al³⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{efn|Partial electrolysis.}}

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=S.J. Patel |title=Aluminium(III) isothiocyanate and its addition compounds |journal=Journal of Inorganic and Nuclear Chemistry |date=1971 |volume=33 |issue=1 |pages=17–22 |doi=10.1016/0022-1902(71)80004-0 |language=en}}

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Gallium Ga³⁺

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=Laurence S. Foster |title=(I) The Reaction of Gallium with Perchloric Acid and (II) the Preparation and Properties of Gallium Perchlorate Hydrates |journal=Journal of the American Chemical Society |date=1939 |volume=61 |issue=11 |pages=3122–3124 |doi=10.1021/ja01266a041 |language=English}}

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=S. J. Patel |author2=D. G. Tuck |title=Gallium(III) isothiocyanate and its addition compounds |journal=Canadian Journal of Chemistry |date=1969 |volume=47 |issue=2 |pages=229–233 |doi=10.1139/v69-032 |language=en}}

| bgcolor="#99CCFF" | S

| ?

align="center"

! Manganese(II) Mn²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite web |title=44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis) |url=https://www.alfa.com/en/catalog/044318/ |website=Alfa Aesar |access-date=16 September 2022}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=B. Beagley |author2=C.A. McAuliffe |author3=A.G. Mackie |author4=R.G. Pritchard |title=Preparation and crystal structure of manganese(II) isothiocyanate tetrahydrate |journal=Inorganica Chimica Acta |date=1984 |volume=89 |issue=3 |pages=163–166 |doi=10.1016/S0020-1693(00)82345-2 |language=en}}

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Iron(II) Fe²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

align="center"

! Cobalt(II) Co²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=E. Kamieńska-Piotrowicz |title=Conductometric Studies of Cobalt(II) Perchlorate in Acetonitrile-Water Solutions |journal=Zeitschrift für Physikalische Chemie |date=1999 |volume=210 |issue=1 |pages=1–13 |doi=10.1524/zpch.1999.210.Part_1.001 |s2cid=102316324 |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Nickel(II) Ni²⁺

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Copper(II) Cu²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| ?

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#FFCCCC" | I{{efn|group=lower-alpha|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.}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Zinc Zn²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=Lili Lin |author2=Xiaohua Liu |author3=Xiaoming Feng |title=Zinc(II) Perchlorate Hexahydrate |journal=Encyclopedia of Reagents for Organic Synthesis |date=2014 |pages=1–5 |doi=10.1002/047084289X.rn01657 |publisher=John Wiley & Sons, Ltd |isbn=9780470842898 |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S{{cite journal |author1=Masaki Kosaku |title=The Solubilities of Thiocyanate of Metals |journal=Bulletin of the Chemical Society of Japan |date=1931 |volume=6 |issue=7 |pages=163–165 |doi=10.1246/bcsj.6.163 |language=en|doi-access=free }}

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Cadmium Cd²⁺

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=P. J. Reilly |author2=R. H. Strokes |title=The diffusion coefficients of cadmium chloride and cadmium perchlorate in water at 25° |journal=Australian Journal of Chemistry |date=1971 |volume=24 |issue=7 |pages=1361–1367 |doi=10.1071/CH9711361 |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Mercury(II) Hg²⁺

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S{{cite journal |author1=Franco Cristiani |author2=Francesco Demartin |author3=Francesco A. Devillanova |author4=Angelo Diaz |author5=Francesco Isaia |author6=Gaetano Verani |title=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=Journal of Coordination Chemistry |date=1990 |volume=21 |issue=2 |pages=137–146 |doi=10.1080/00958979009409182 |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS{{cite web |title=Properties of substance: mercury(II) oxalate Group of substances |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=2631 |website=Chemister |access-date=13 September 2022 |language=English}}

align="center"

! Vanadium(III) V³⁺

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=Burkhart, M J |author2=Newton, T W |title=Kinetics of the reaction between vanadium(II) and neptunium(IV) in aqueous perchlorate solutions |journal=J. Phys. Chem. |date=1969 |volume=73 |issue=6 |pages=1741–1746 |doi=10.1021/j100726a018 |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| ?

| bgcolor="#99CCFF" | S

| ?

align="center"

! Chromium(III) Cr³⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| ?

align="center"

! Iron(III) Fe³⁺

| bgcolor="#99CCFF" | S{{efn|group=lower-alpha|Anhydrous FeF₃ is slightly soluble in water; FeF₃·3H₂O is much more soluble in water.}}

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S{{cite journal |author1=M. Magini |title=An X-ray investigation on the structure of iron(III) perchlorate solutions |journal=Journal of Inorganic and Nuclear Chemistry |date=1978 |volume=40 |issue=1 |pages=43–48 |doi=10.1016/0022-1902(78)80304-2 |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| bgcolor="#CCCCCC" | R{{Cite web |title=Iron (III) Carbonate Formula |website=softschools.com |access-date=19 August 2022 |pages = 1|url=https://www.softschools.com/formulas/chemistry/iron_iii_carbonate_formula/670/#:~:text=Iron%20(III)%20carbonate%2C%20also,is%20291.72%20g%20mol%2D1.}}

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=Sano Hirotoshi |author2=Akane Michiko |title=MÖSSBAUER SPECTROSCOPIC STUDIES ON IRON THIOCYANATE |journal=Chemistry Letters |date=1973 |volume=2 |issue=1 |pages=43–46 |doi=10.1246/cl.1973.43 |language=en}}

| bgcolor="#99CCFF" | S{{cite journal |author1=Ram C. Paul |author2=Ramesh C. Narula |author3=Sham K. Vasisht |title=Iron(III) acetates |journal=Transition Metal Chemistry |date=1978 |volume=3 |pages=35–38 |doi=10.1007/BF01393501 |s2cid=94447648 |language=en}}{{efn|group=lower-alpha|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.}}

| bgcolor="#CCCCFF" | sS

align="center"

! Gold(III) Au³⁺

| bgcolor="#CCCCCC" | R

| bgcolor="#99CCFF" | S

| bgcolor="#CCCCFF" | sS

| ?

| bgcolor="#FFCCCC" | I

| ?

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| ?

| bgcolor="#CCCCFF" | sS

| ?

align="center"

! Tin(II) Sn²⁺

| bgcolor="#99CCFF" | S

| bgcolor="#99CCFF" | S{{cite journal |author1=C.G.Davies |author2=J.D.Donaldson |title=Tin(II) perchlorate trihydrate |journal=Journal of Inorganic and Nuclear Chemistry |date=1968 |volume=30 |issue=10 |pages=2635–2639 |doi=10.1016/0022-1902(68)80389-6 |location=Chelsea College of Science and Technology |language=en}}

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| ?

| bgcolor="#FFCCCC" | I

| ?

| bgcolor="#FFCCCC" | I{{cite journal |author1=Tewfik B. Absi |author2=Ramesh C. Makhija |author3=Mario Onyszchuk |title=Synthesis and vibrational spectra of tin(II) isothiocyanate adducts with some O- and N-donor ligands |journal=Canadian Journal of Chemistry |date=1978 |volume=56 |issue=15 |pages=2039–2041 |doi=10.1139/v78-333 |language=English}}

| bgcolor="#CCCCCC" | R

| bgcolor="#CCCCFF" | sS

align="center"

! Lead(II) Pb²⁺

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

align="center"

! Silver Ag⁺

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S

| bgcolor="#FFCCCC" | I

| bgcolor="#CCCCFF" | sS

| bgcolor="#FFCCCC" | I

align="center"

! Mercury(I) {{chem|Hg|2|2+}}

| bgcolor="#CCCCCC" | R

| bgcolor="#FFCCCC" | I

| bgcolor="#99CCFF" | S{{cite journal |author1=D. R. Rossėinsky |title=The reaction between mercury(I) and manganese(III) in aqueous perchlorate solution |journal=Journal of the Chemical Society (Resumed) |date=1963 |pages=1181–1186 |doi=10.1039/JR9630001181 |language=en}}

| bgcolor="#FFCCCC" | I

| ?

| bgcolor="#CCCCFF" | sS

| bgcolor="#99CCFF" | S{{efn|name=MercurousSlowReact|group=lower-alpha|Slowly decomposes in water.}}

| ?

| bgcolor="#FFCCCC" | I

| ?

| bgcolor="#99CCFF" | S{{cite web |last1=National Center for Biotechnology Information |title=PubChem Compound Summary for CID 61181, Mercurous acetate |url=https://pubchem.ncbi.nlm.nih.gov/compound/Mercurous-acetate |website=PubChem}}{{efn|name=MercurousSlowReact}}

| ?

width="5.88%" |

! width="5.88%" | Fluoride
F⁻

! width="5.88%" | Chloride
Cl⁻

! width="5.88%" | Bromide
Br⁻

! width="5.88%" | Iodide
I⁻

! width="5.88%" | Perchlorate
{{chem|ClO|4|−}}

! width="5.88%" | Oxide
O²⁻

! width="5.88%" | Hydroxide
OH⁻

! width="5.88%" | Sulfide
S²⁻

! width="5.88%" | Sulfate
{{chem|SO|4|2−}}

! width="5.88%" | Nitrate
{{chem|NO|3|−}}{{efn|name=AlwaysSolubleK}}

! width="5.88%" | Phosphate
{{chem|PO|4|3−}}

! width="5.88%" | Carbonate
{{chem|CO|3|2−}}{{efn|name=AlwaysSolubleK}}

! width="5.88%" | Cyanide
CN⁻

! width="5.88%" | Thiocyanate
SCN⁻

! width="5.88%" | Acetate
{{chem|C|2|H|3|O|2|−}}

! width="5.88%" | Oxalate
{{chem|C|2|O|4|2−}}

Notes

References

Category:Solutions

Solubility chart

Chart

See also

Notes

References