# Solubility chart > Mediated Wiki article. Canonical URL: https://mediated.wiki/source/Solubility_chart > Markdown URL: https://mediated.wiki/source/Solubility_chart.md > Source: https://en.wikipedia.org/wiki/Solubility_chart > Source revision: 1352261483 > License: Creative Commons Attribution-ShareAlike 4.0 International (https://creativecommons.org/licenses/by-sa/4.0/) {{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](/source/ionic_compounds) formed from different combinations of [cations and anions](/source/ion) dissolve in or [precipitate](/source/precipitation_(chemistry)) from solution. ==Chart== The following chart shows the [solubility](/source/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 does not precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like [calcium sulfate](/source/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](/source/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" |[Halogen](/source/Halogen)s ! colspan="4" |[Chalcogen](/source/Chalcogen)s ! colspan="3" |[Pnictogen](/source/Pnictogen)s ! colspan="5" |[Crystallogens](/source/Carbon_group) |- ! [Fluoride](/source/Fluoride)
F− ! [Chloride](/source/Chloride)
Cl− ! [Bromide](/source/Bromide)
Br− ! [Iodide](/source/Iodide)
I− ! [Perchlorate](/source/Perchlorate)
{{chem|ClO|4|−}} ! [Oxide](/source/Oxide)
O2− ! [Hydroxide](/source/Hydroxide)
OH− ! [Sulfide](/source/Sulfide)
S2− ! [Sulfate](/source/Sulfate)
{{chem|SO|4|2−}} ! [Nitrate](/source/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](/source/Alkali_metal) elements or ammonium.{{cite web |url=http://intro.chem.okstate.edu/1515SP01/Database/Solub.html |title=Solubility Table |website=intro.chem.okstate.edu}}}} ! [Azide](/source/Azide)
{{chem|N|3|−}} ! [Phosphate](/source/Phosphate)
{{chem|PO|4|3−}} ! [Carbonate](/source/Carbonate)
{{chem|CO|3|2−}}{{efn|name=AlwaysSolubleK}} ! [Cyanide](/source/Cyanide)
CN− ! [Thiocyanate](/source/Thiocyanate)
SCN− ! [Acetate](/source/Acetate)
{{chem|C|2|H|3|O|2|−}} ! [Oxalate](/source/Oxalate)
{{chem|C|2|O|4|2−}} |- align="center" ! [Hydrogen](/source/Hydrogen) H+ | bgcolor="#99CCFF" | [S](/source/Hydrogen_fluoride) | bgcolor="#99CCFF" | [S](/source/Hydrogen_chloride) | bgcolor="#99CCFF" | [S](/source/Hydrogen_bromide) | bgcolor="#99CCFF" | [S](/source/Hydrogen_iodide) | bgcolor="#99CCFF" | [S](/source/Perchloric_acid) | N/A | N/A | bgcolor="#CCCCFF" | [sS](/source/Hydrogen_sulfide) | bgcolor="#99CCFF" | [S](/source/Sulfuric_acid) | bgcolor="#99CCFF" | [S](/source/Hydrogen_nitrate) | bgcolor="#99CCFF" | [S](/source/Hydrazoic_acid) | bgcolor="#99CCFF" | [S](/source/Phosphoric_acid) | bgcolor="#99CCFF" | [S](/source/Carbonic_acid) | bgcolor="#99CCFF" | [S](/source/Hydrogen_cyanide) | bgcolor="#99CCFF" | [S](/source/Thiocyanic_acid) | bgcolor="#99CCFF" | [S](/source/Acetic_acid) | bgcolor="#99CCFF" | [S](/source/Oxalic_acid) |- align="center" ! [Ammonium](/source/Ammonium) {{chem|NH|4|+}}{{efn|name=AlwaysSolubleK}} | bgcolor="#99CCFF" | [S](/source/Ammonium_fluoride) | bgcolor="#99CCFF" | [S](/source/Ammonium_chloride) | bgcolor="#99CCFF" | [S](/source/Ammonium_bromide) | bgcolor="#99CCFF" | [S](/source/Ammonium_iodide) | bgcolor="#99CCFF" | [S](/source/Ammonium_perchlorate) | bgcolor="#99CCFF" | [S](/source/Ammonium_hydroxide){{efn|group=lower-alpha|"Ammonium oxide" does not exist. However, its theoretical molecular formula ({{chem|NH|4|+}})2O2− represents that of [aqueous ammonia](/source/Ammonia_solution).}} | bgcolor="#99CCFF" | [S](/source/Ammonium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Ammonium_sulfide) | bgcolor="#99CCFF" | [S](/source/Ammonium_sulfate) | bgcolor="#99CCFF" | [S](/source/Ammonium_nitrate) | bgcolor="#99CCFF" | [S](/source/Ammonium_azide) | bgcolor="#99CCFF" | [S](/source/Ammonium_phosphate) | bgcolor="#99CCFF" | [S](/source/Ammonium_carbonate) | bgcolor="#99CCFF" | [S](/source/Ammonium_cyanide) | bgcolor="#99CCFF" | [S](/source/Ammonium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Ammonium_acetate) | bgcolor="#99CCFF" | [S](/source/Ammonium_oxalate) |- align="center" ! [Lithium](/source/Lithium) Li+ | bgcolor="#CCCCFF" | [sS](/source/Lithium_fluoride) | bgcolor="#99CCFF" | [S](/source/Lithium_chloride) | bgcolor="#99CCFF" | [S](/source/Lithium_bromide) | bgcolor="#99CCFF" | [S](/source/Lithium_iodide) | bgcolor="#99CCFF" | [S](/source/Lithium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Lithium_oxide) | bgcolor="#99CCFF" | [S](/source/Lithium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Lithium_sulfide) | bgcolor="#99CCFF" | [S](/source/Lithium_sulfate) | bgcolor="#99CCFF" | [S](/source/Lithium_nitrate) | bgcolor="#99CCFF" | [S](/source/Lithium_azide) | bgcolor="#CCCCFF" | [sS](/source/Lithium_phosphate) | bgcolor="#CCCCFF" | [sS](/source/Lithium_carbonate) | bgcolor="#99CCFF" | [S](/source/Lithium_cyanide) | bgcolor="#99CCFF" | [S](/source/Lithium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Lithium_acetate) | bgcolor="#99CCFF" | [S](/source/Lithium_oxalate) |- align="center" ! [Sodium](/source/Sodium) Na+ | bgcolor="#99CCFF" | [S](/source/Sodium_fluoride) | bgcolor="#99CCFF" | [S](/source/Sodium_chloride) | bgcolor="#99CCFF" | [S](/source/Sodium_bromide) | bgcolor="#99CCFF" | [S](/source/Sodium_iodide) | bgcolor="#99CCFF" | [S](/source/Sodium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Sodium_oxide) | bgcolor="#99CCFF" | [S](/source/Sodium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Sodium_sulfide) | bgcolor="#99CCFF" | [S](/source/Sodium_sulfate) | bgcolor="#99CCFF" | [S](/source/Sodium_nitrate) | bgcolor="#99CCFF" | [S](/source/Sodium_azide) | bgcolor="#99CCFF" | [S](/source/Trisodium_phosphate) | bgcolor="#99CCFF" | [S](/source/Sodium_carbonate) | bgcolor="#99CCFF" | [S](/source/Sodium_cyanide) | bgcolor="#99CCFF" | [S](/source/Sodium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Sodium_acetate) | bgcolor="#99CCFF" | [S](/source/Sodium_oxalate) |- align="center" ! [Potassium](/source/Potassium) K+ | bgcolor="#99CCFF" | [S](/source/Potassium_fluoride) | bgcolor="#99CCFF" | [S](/source/Potassium_chloride) | bgcolor="#99CCFF" | [S](/source/Potassium_bromide) | bgcolor="#99CCFF" | [S](/source/Potassium_iodide) | bgcolor="#CCCCFF" | [sS](/source/Potassium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Potassium_oxide) | bgcolor="#99CCFF" | [S](/source/Potassium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Potassium_sulfide) | bgcolor="#99CCFF" | [S](/source/Potassium_sulfate) | bgcolor="#99CCFF" | [S](/source/Potassium_nitrate) | bgcolor="#99CCFF" | [S](/source/Potassium_azide) | bgcolor="#99CCFF" | [S](/source/Tripotassium_phosphate) | bgcolor="#99CCFF" | [S](/source/Potassium_carbonate) | bgcolor="#99CCFF" | [S](/source/Potassium_cyanide) | bgcolor="#99CCFF" | [S](/source/Potassium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Potassium_acetate) | bgcolor="#99CCFF" | [S](/source/Potassium_oxalate) |- align="center" ! [Rubidium](/source/Rubidium) Rb+ | bgcolor="#99CCFF" | [S](/source/Rubidium_fluoride) | bgcolor="#99CCFF" | [S](/source/Rubidium_chloride) | bgcolor="#99CCFF" | [S](/source/Rubidium_bromide) | bgcolor="#99CCFF" | [S](/source/Rubidium_iodide) | bgcolor="#CCCCFF" | [sS](/source/Rubidium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Rubidium_oxide) | bgcolor="#99CCFF" | [S](/source/Rubidium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Rubidium_sulfide) | bgcolor="#99CCFF" | [S](/source/Rubidium_sulfate) | bgcolor="#99CCFF" | [S](/source/Rubidium_nitrate) | bgcolor="#99CCFF" | [S](/source/Rubidium_azide) | bgcolor="#99CCFF" | [S](/source/Rubidium_phosphate) | bgcolor="#99CCFF" | [S](/source/Rubidium_carbonate) | bgcolor="#99CCFF" | [S](/source/Rubidium_cyanide) | bgcolor="#99CCFF" | [S](/source/Rubidium_thiocyanate){{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](/source/Rubidium_acetate) | bgcolor="#99CCFF" | [S](/source/Rubidium_oxalate) |- align="center" ! [Caesium](/source/Caesium) Cs+ | bgcolor="#99CCFF" | [S](/source/Caesium_fluoride) | bgcolor="#99CCFF" | [S](/source/Caesium_chloride) | bgcolor="#99CCFF" | [S](/source/Caesium_bromide) | bgcolor="#99CCFF" | [S](/source/Caesium_iodide) | bgcolor="#CCCCFF" | [sS](/source/Caesium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Caesium_oxide) | bgcolor="#99CCFF" | [S](/source/Caesium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Caesium_sulfide) | bgcolor="#99CCFF" | [S](/source/Caesium_sulfate) | bgcolor="#99CCFF" | [S](/source/Caesium_nitrate) | bgcolor="#99CCFF" | [S](/source/Caesium_azide) | bgcolor="#99CCFF" | [S](/source/Caesium_phosphate) | bgcolor="#99CCFF" | [S](/source/Caesium_carbonate) | bgcolor="#99CCFF" | [S](/source/Caesium_cyanide) | bgcolor="#99CCFF" | [S](/source/Caesium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Caesium_acetate) | bgcolor="#99CCFF" | [S](/source/Caesium_oxalate) |- align="center" ! [Beryllium](/source/Beryllium) Be2+ | bgcolor="#99CCFF" | [S](/source/Beryllium_fluoride) | bgcolor="#99CCFF" | [S](/source/Beryllium_chloride) | bgcolor="#99CCFF" | [S](/source/Beryllium_bromide) | bgcolor="#CCCCCC" | [R](/source/Beryllium_iodide) | bgcolor="#99CCFF" | [S](/source/Beryllium_perchlorate){{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](/source/Beryllium_oxide) | bgcolor="#FFCCCC" | [I](/source/Beryllium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Beryllium_sulfide) | bgcolor="#99CCFF" | [S](/source/Beryllium_sulfate) | bgcolor="#99CCFF" | [S](/source/Beryllium_nitrate) | bgcolor="#CCCCCC" | [R](/source/Beryllium_azide) | bgcolor="#FFCCCC" | [I](/source/Beryllium_phosphate) | bgcolor="#CCCCFF" | [sS](/source/Beryllium_carbonate) | bgcolor="#CCCCCC" | [R](/source/Beryllium_cyanide) | bgcolor="#99CCFF" | [S](/source/Beryllium_thiocyanate){{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](/source/Beryllium_acetate) | bgcolor="#99CCFF" | [S](/source/Beryllium_oxalate) |- align="center" ! [Magnesium](/source/Magnesium) Mg2+ | bgcolor="#CCCCFF" | [sS](/source/Magnesium_fluoride) | bgcolor="#99CCFF" | [S](/source/Magnesium_chloride) | bgcolor="#99CCFF" | [S](/source/Magnesium_bromide) | bgcolor="#99CCFF" | [S](/source/Magnesium_iodide) | bgcolor="#99CCFF" | [S](/source/Magnesium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Magnesium_oxide) | bgcolor="#FFCCCC" | [I](/source/Magnesium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Magnesium_sulfide) | bgcolor="#99CCFF" | [S](/source/Magnesium_sulfate) | bgcolor="#99CCFF" | [S](/source/Magnesium_nitrate) | bgcolor="#CCCCCC" | [R](/source/Magnesium_azide) | bgcolor="#FFCCCC" | [I](/source/Trimagnesium_phosphate) | bgcolor="#CCCCFF" | [sS](/source/Magnesium_carbonate) | bgcolor="#CCCCCC" | [R](/source/Magnesium_cyanide) | bgcolor="#99CCFF" | [S](/source/Magnesium_thiocyanate){{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](/source/Magnesium_acetate) | bgcolor="#CCCCFF" | [sS](/source/Magnesium_oxalate) |- align="center" ! [Calcium](/source/Calcium) Ca2+ | bgcolor="#FFCCCC" | [I](/source/Calcium_fluoride) | bgcolor="#99CCFF" | [S](/source/Calcium_chloride) | bgcolor="#99CCFF" | [S](/source/Calcium_bromide) | bgcolor="#99CCFF" | [S](/source/Calcium_iodide) | bgcolor="#99CCFF" | [S](/source/Calcium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Calcium_oxide) | bgcolor="#CCCCFF" | [sS](/source/Calcium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Calcium_sulfide) | bgcolor="#CCCCFF" | [sS](/source/Calcium_sulfate) | bgcolor="#99CCFF" | [S](/source/Calcium_nitrate) | bgcolor="#99CCFF" | [S](/source/Calcium_azide) | bgcolor="#FFCCCC" | [I](/source/Tricalcium_phosphate) | bgcolor="#FFCCCC" | [I](/source/Calcium_carbonate) | bgcolor="#CCCCCC" | [R](/source/Calcium_cyanide) | bgcolor="#99CCFF" | [S](/source/Calcium_thiocyanate){{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](/source/Calcium_acetate) | bgcolor="#CCCCFF" | [sS](/source/Calcium_oxalate) |- align="center" ! [Strontium](/source/Strontium) Sr2+ | bgcolor="#CCCCFF" | [sS](/source/Strontium_fluoride) | bgcolor="#99CCFF" | [S](/source/Strontium_chloride) | bgcolor="#99CCFF" | [S](/source/Strontium_bromide) | bgcolor="#99CCFF" | [S](/source/Strontium_iodide) | bgcolor="#99CCFF" | [S](/source/Strontium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Strontium_oxide) | bgcolor="#CCCCFF" | [sS](/source/Strontium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Strontium_sulfide) | bgcolor="#CCCCFF" | [sS](/source/Strontium_sulfate) | bgcolor="#99CCFF" | [S](/source/Strontium_nitrate) | bgcolor="#99CCFF" | [S](/source/Strontium_azide) | bgcolor="#FFCCCC" | [I](/source/Strontium_phosphate) | bgcolor="#FFCCCC" | [I](/source/Strontium_carbonate) | bgcolor="#99CCFF" | [S](/source/Strontium_cyanide) | bgcolor="#99CCFF" | [S](/source/Strontium_thiocyanate){{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](/source/Strontium_acetate) | bgcolor="#FFCCCC" | [I](/source/Strontium_oxalate) |- align="center" ! [Barium](/source/Barium) Ba2+ | bgcolor="#CCCCFF" | [sS](/source/Barium_fluoride) | bgcolor="#99CCFF" | [S](/source/Barium_chloride) | bgcolor="#99CCFF" | [S](/source/Barium_bromide) | bgcolor="#99CCFF" | [S](/source/Barium_iodide) | bgcolor="#99CCFF" | [S](/source/Barium_perchlorate) | bgcolor="#CCCCCC" | [R](/source/Barium_oxide) | bgcolor="#99CCFF" | [S](/source/Barium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Barium_sulfide) | bgcolor="#FFCCCC" | [I](/source/Barium_sulfate) | bgcolor="#99CCFF" | [S](/source/Barium_nitrate) | bgcolor="#99CCFF" | [S](/source/Barium_azide) | bgcolor="#FFCCCC" | [I](/source/Barium_phosphate){{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="#FFCCCC" | [I](/source/Barium_carbonate) | bgcolor="#99CCFF" | [S](/source/Barium_cyanide) | bgcolor="#99CCFF" | [S](/source/Barium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Barium_acetate) | bgcolor="#FFCCCC" | [I](/source/Barium_oxalate) |- align="center" ! [Aluminium](/source/Aluminium) Al3+ | bgcolor="#CCCCFF" | [sS](/source/Aluminium_fluoride) | bgcolor="#99CCFF" | [S](/source/Aluminium_chloride) | bgcolor="#99CCFF" | [S](/source/Aluminium_bromide) | bgcolor="#99CCFF" | [S](/source/Aluminium_iodide){{efn|Partial electrolysis.}} | bgcolor="#99CCFF" | [S](/source/Aluminium_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Aluminium_oxide) | bgcolor="#FFCCCC" | [I](/source/Aluminium_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Aluminium_sulfide) | bgcolor="#99CCFF" | [S](/source/Aluminium_sulfate) | bgcolor="#99CCFF" | [S](/source/Aluminium_nitrate) | bgcolor="#CCCCCC" | [R](/source/Aluminium_azide) | bgcolor="#FFCCCC" | [I](/source/Aluminium_phosphate) | bgcolor="#CCCCCC" | [R](/source/Aluminium_carbonate) | bgcolor="#CCCCCC" | [R](/source/Aluminium_cyanide) | bgcolor="#99CCFF" | [S](/source/Aluminium_thiocyanate){{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](/source/Aluminium_triacetate) | bgcolor="#FFCCCC" | [I](/source/Aluminium_oxalate) |- align="center" ! [Gallium](/source/Gallium) Ga3+ | bgcolor="#FFCCCC" | [I](/source/Gallium_fluoride) | bgcolor="#99CCFF" | [S](/source/Gallium_trichloride) | bgcolor="#99CCFF" | [S](/source/Gallium_bromide) | bgcolor="#CCCCCC" | [R](/source/Gallium_iodide) | bgcolor="#99CCFF" | [S](/source/Gallium_perchlorate){{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](/source/Gallium(III)_oxide) | bgcolor="#FFCCCC" | [I](/source/Gallium(III)_hydroxide) | bgcolor="#CCCCCC" | [R](/source/Gallium(III)_sulfide) | bgcolor="#CCCCFF" | [sS](/source/Gallium(III)_sulfate) | bgcolor="#99CCFF" | [S](/source/Gallium_nitrate) | bgcolor="#CCCCCC" | [R](/source/Gallium_azide) | bgcolor="#FFCCCC" | [I](/source/Gallium_phosphate) | bgcolor="#CCCCCC" | [R](/source/Gallium_carbonate) | bgcolor="#CCCCCC" | [R](/source/Gallium(III)_cyanide) | bgcolor="#99CCFF" | [S](/source/Gallium_thiocyanate){{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](/source/Gallium_acetate) | ? |- align="center" ! [Manganese](/source/Manganese)(II) Mn2+ | bgcolor="#CCCCFF" | [sS](/source/Manganese(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_chloride) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_bromide) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_perchlorate){{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](/source/Manganese(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Manganese(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Manganese(II)_sulfide) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_nitrate) | bgcolor="#CCCCCC" | [R](/source/Manganese(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Manganese(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Manganese(II)_carbonate) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_cyanide) | bgcolor="#99CCFF" | [S](/source/Manganese(II)_thiocyanate){{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](/source/Manganese(II)_acetate) | bgcolor="#FFCCCC" | [I](/source/Manganese(II)_oxalate) |- align="center" ! [Iron](/source/Iron)(II) Fe2+ | bgcolor="#CCCCFF" | [sS](/source/Iron(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Iron(II)_chloride) | bgcolor="#99CCFF" | [S](/source/Iron(II)_bromide) | bgcolor="#99CCFF" | [S](/source/Iron(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Iron(II)_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Iron(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Iron(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Iron(II)_sulfide) | bgcolor="#99CCFF" | [S](/source/Iron(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Iron(II)_nitrate) | ? | bgcolor="#FFCCCC" | [I](/source/Iron(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Iron(II)_carbonate) | [?](/source/Iron(II)_cyanide) | bgcolor="#99CCFF" | [S](/source/Iron(II)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Iron(II)_acetate) | bgcolor="#CCCCFF" | [sS](/source/Iron(II)_oxalate) |- align="center" ! [Cobalt](/source/Cobalt)(II) Co2+ | bgcolor="#CCCCFF" | [sS](/source/Cobalt(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_chloride) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_bromide) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_perchlorate){{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](/source/Cobalt(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Cobalt(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Cobalt_sulfide) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_nitrate) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Cobalt(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Cobalt(II)_carbonate) | bgcolor="#FFCCCC" | [I](/source/Cobalt(II)_cyanide) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Cobalt(II)_acetate) | bgcolor="#FFCCCC" | [I](/source/Cobalt(II)_oxalate) |- align="center" ! [Nickel](/source/Nickel)(II) Ni2+ | bgcolor="#99CCFF" | [S](/source/Nickel(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_chloride) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_bromide) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Nickel(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Nickel(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Nickel_sulfide) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_nitrate) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Nickel(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Nickel(II)_carbonate) | bgcolor="#FFCCCC" | [I](/source/Nickel(II)_cyanide) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Nickel(II)_acetate) | bgcolor="#FFCCCC" | [I](/source/Nickel(II)_oxalate) |- align="center" ! [Copper](/source/Copper)(II) Cu2+ | bgcolor="#CCCCFF" | [sS](/source/Copper(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Copper(II)_chloride) | bgcolor="#99CCFF" | [S](/source/Copper(II)_bromide) | ? | bgcolor="#99CCFF" | [S](/source/Copper(II)_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_sulfide) | bgcolor="#99CCFF" | [S](/source/Copper(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Copper(II)_nitrate) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_carbonate){{efn|group=lower-alpha|The commonly encountered [basic copper carbonate](/source/basic_copper_carbonate) (Cu2CO3(OH)2) is insoluble in water. True [copper(II) carbonate](/source/copper(II)_carbonate) (CuCO3) is rare and reacts with water to form basic copper carbonate.}} | bgcolor="#FFCCCC" | [I](/source/Copper(II)_cyanide) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Copper(II)_acetate) | bgcolor="#FFCCCC" | [I](/source/Copper(II)_oxalate) |- align="center" ! [Zinc](/source/Zinc) Zn2+ | bgcolor="#CCCCFF" | [sS](/source/Zinc_fluoride) | bgcolor="#99CCFF" | [S](/source/Zinc_chloride) | bgcolor="#99CCFF" | [S](/source/Zinc_bromide) | bgcolor="#99CCFF" | [S](/source/zinc_iodide) | bgcolor="#99CCFF" | [S](/source/Zinc_perchlorate){{cite book |author1=Lili Lin |author2=Xiaohua Liu |author3=Xiaoming Feng |chapter=Zinc(II) Perchlorate Hexahydrate |title=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](/source/Zinc_oxide) | bgcolor="#FFCCCC" | [I](/source/Zinc_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Zinc_sulfide) | bgcolor="#99CCFF" | [S](/source/Zinc_sulfate) | bgcolor="#99CCFF" | [S](/source/Zinc_nitrate) | bgcolor="#CCCCCC" | [R](/source/Zinc_azide) | bgcolor="#FFCCCC" | [I](/source/Zinc_phosphate) | bgcolor="#FFCCCC" | [I](/source/Zinc_carbonate) | bgcolor="#FFCCCC" | [I](/source/Zinc_cyanide) | bgcolor="#99CCFF" | [S](/source/Zinc_thiocyanate){{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](/source/Zinc_acetate) | bgcolor="#FFCCCC" | [I](/source/Zinc_oxalate) |- align="center" ! [Cadmium](/source/Cadmium) Cd2+ | bgcolor="#99CCFF" | [S](/source/Cadmium_fluoride) | bgcolor="#99CCFF" | [S](/source/Cadmium_chloride) | bgcolor="#99CCFF" | [S](/source/Cadmium_bromide) | bgcolor="#99CCFF" | [S](/source/Cadmium_iodide) | bgcolor="#99CCFF" | [S](/source/Cadmium_perchlorate){{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](/source/Cadmium_oxide) | bgcolor="#FFCCCC" | [I](/source/Cadmium_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Cadmium_sulfide) | bgcolor="#99CCFF" | [S](/source/Cadmium_sulfate) | bgcolor="#99CCFF" | [S](/source/Cadmium_nitrate) | bgcolor="#99CCFF" | [S](/source/Cadmium_azide) | bgcolor="#FFCCCC" | [I](/source/Cadmium_phosphate) | bgcolor="#FFCCCC" | [I](/source/Cadmium_carbonate) | bgcolor="#CCCCFF" | [sS](/source/Cadmium_cyanide) | bgcolor="#CCCCFF" | [sS](/source/Cadmium_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Cadmium_acetate) | bgcolor="#FFCCCC" | [I](/source/Cadmium_oxalate) |- align="center" ! [Mercury](/source/Mercury_(element))(II) Hg2+ | bgcolor="#CCCCCC" | [R](/source/Mercury(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Mercury(II)_chloride) | bgcolor="#CCCCFF" | [sS](/source/Mercury(II)_bromide) | bgcolor="#FFCCCC" | [I](/source/Mercury(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Mercury(II)_perchlorate){{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](/source/Mercury(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Mercury(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Mercury_sulfide) | bgcolor="#CCCCCC" | [R](/source/Mercury(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Mercury(II)_nitrate) | bgcolor="#CCCCFF" | [sS](/source/Mercury(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Mercury(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Mercury(II)_carbonate) | bgcolor="#99CCFF" | [S](/source/Mercury(II)_cyanide) | bgcolor="#CCCCFF" | [sS](/source/Mercury(II)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Mercury(II)_acetate) | bgcolor="#CCCCFF" | [sS](/source/Mercury(II)_oxalate){{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](/source/Vanadium)(III) V3+ | bgcolor="#FFCCCC" | [I](/source/Vanadium(III)_fluoride) | bgcolor="#99CCFF" | [S](/source/Vanadium(III)_chloride) | bgcolor="#99CCFF" | [S](/source/Vanadium(III)_bromide) | bgcolor="#99CCFF" | [S](/source/Vanadium(III)_iodide) | bgcolor="#99CCFF" | [S](/source/Vanadium(III)_perchlorate){{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](/source/Vanadium(III)_oxide) | bgcolor="#FFCCCC" | [I](/source/Vanadium(III)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Vanadium(III)_sulfide) | bgcolor="#CCCCFF" | [sS](/source/Vanadium(III)_sulfate) | bgcolor="#99CCFF" | [S](/source/Vanadium(III)_nitrate) | ? | bgcolor="#FFCCCC" | [I](/source/Vanadium_phosphate) | ? | ? | bgcolor="#99CCFF" | [S](/source/Vanadium(III)_thiocyanate) | ? | ? |- align="center" ! [Chromium](/source/Chromium)(III) Cr3+ | bgcolor="#CCCCFF" | [sS](/source/Chromium(III)_fluoride) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_chloride) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_bromide) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_iodide) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Chromium(III)_oxide) | bgcolor="#FFCCCC" | [I](/source/Chromium(III)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Chromium(III)_sulfide) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_sulfate) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_nitrate) | bgcolor="#CCCCCC" | [R](/source/Chromium(III)_azide) | bgcolor="#FFCCCC" | [I](/source/Chromium(III)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Chromium(III)_carbonate) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_cyanide) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Chromium(III)_acetate) | ? |- align="center" ! [Iron](/source/Iron)(III) Fe3+ | bgcolor="#99CCFF" | [S](/source/Iron(III)_fluoride){{efn|group=lower-alpha|Anhydrous FeF3 is slightly soluble in water; FeF3·3H2O is much more soluble in water.}} | bgcolor="#99CCFF" | [S](/source/Iron(III)_chloride) | bgcolor="#99CCFF" | [S](/source/Iron(III)_bromide) | bgcolor="#CCCCCC" | [R](/source/Iron(III)_iodide) | bgcolor="#99CCFF" | [S](/source/Iron(III)_perchlorate){{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](/source/Iron(III)_oxide) | bgcolor="#FFCCCC" | [I](/source/Iron(III)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Iron(III)_sulfide) | bgcolor="#99CCFF" | [S](/source/Iron(III)_sulfate) | bgcolor="#99CCFF" | [S](/source/Iron(III)_nitrate) | bgcolor="#99CCFF" | [S](/source/Iron(III)_azide) | bgcolor="#CCCCFF" | [sS](/source/Iron(III)_phosphate) | bgcolor="#CCCCCC" | [R](/source/Iron(III)_carbonate){{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](/source/Iron(III)_cyanide) | bgcolor="#99CCFF" | [S](/source/Iron(III)_thiocyanate){{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](/source/Iron(III)_acetate){{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](/source/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](/source/Iron(III)_oxalate) |- align="center" ! [Gold](/source/Gold)(III) Au3+ | bgcolor="#CCCCCC" | [R](/source/Gold(III)_fluoride) | bgcolor="#99CCFF" | [S](/source/Gold(III)_chloride) | bgcolor="#CCCCFF" | [sS](/source/Gold(III)_bromide) | [?](/source/Gold(III)_iodide) | ? | bgcolor="#FFCCCC" | [I](/source/Gold(III)_oxide) | bgcolor="#FFCCCC" | [I](/source/Gold(III)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Gold(III)_sulfide) | ? | ? | ? | bgcolor="#FFCCCC" | [I](/source/Gold(III)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Gold(III)_carbonate) | bgcolor="#99CCFF" | [S](/source/Auric_cyanide) | ? | bgcolor="#CCCCFF" | [sS](/source/Gold(III)_acetate) | ? |- align="center" ! [Tin](/source/Tin)(II) Sn2+ | bgcolor="#99CCFF" | [S](/source/Tin(II)_fluoride) | bgcolor="#99CCFF" | [S](/source/Tin(II)_chloride) | bgcolor="#99CCFF" | [S](/source/Tin(II)_bromide) | bgcolor="#99CCFF" | [S](/source/Tin(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Tin(II)_perchlorate){{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](/source/Tin(II)_oxide) | bgcolor="#FFCCCC" | [I](/source/Tin(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Tin(II)_sulfide) | bgcolor="#99CCFF" | [S](/source/Tin(II)_sulfate) | ? | bgcolor="#CCCCFF" | [sS](/source/Tin(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Tin(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Tin(II)_carbonate) | ? | bgcolor="#FFCCCC" | [I](/source/Tin(II)_thiocyanate){{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](/source/Tin(II)_acetate) | bgcolor="#CCCCFF" | [sS](/source/Tin(II)_oxalate) |- align="center" ! [Lead](/source/Lead)(II) Pb2+ | bgcolor="#CCCCFF" | [sS](/source/Lead(II)_fluoride) | bgcolor="#CCCCFF" | [sS](/source/Lead(II)_chloride) | bgcolor="#CCCCFF" | [sS](/source/Lead(II)_bromide) | bgcolor="#CCCCFF" | [sS](/source/Lead(II)_iodide) | bgcolor="#99CCFF" | [S](/source/Lead(II)_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Lead(II)_oxide) | bgcolor="#CCCCFF" | [sS](/source/Lead(II)_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Lead(II)_sulfide) | bgcolor="#FFCCCC" | [I](/source/Lead(II)_sulfate) | bgcolor="#99CCFF" | [S](/source/Lead(II)_nitrate) | bgcolor="#99CCFF" | [S](/source/Lead(II)_azide) | bgcolor="#FFCCCC" | [I](/source/Lead(II)_phosphate) | bgcolor="#FFCCCC" | [I](/source/Lead(II)_carbonate) | ?{{cite journal | last1=Schulz | first1=Axel | last2=Surkau | first2=Jonas | title=Main group cyanides: from hydrogen cyanide to cyanido-complexes | journal=Reviews in Inorganic Chemistry | volume=43 | issue=1 | date=2023 | issn=0193-4929 | doi=10.1515/revic-2021-0044 | doi-access=free | pages=49–188 }} | bgcolor="#CCCCFF" | [sS](/source/Lead(II)_thiocyanate) | bgcolor="#99CCFF" | [S](/source/Lead(II)_acetate) | bgcolor="#FFCCCC" | [I](/source/Lead(II)_oxalate) |- align="center" ! [Silver](/source/Silver) Ag+ | bgcolor="#99CCFF" | [S](/source/Silver(I)_fluoride) | bgcolor="#FFCCCC" | [I](/source/Silver_chloride) | bgcolor="#FFCCCC" | [I](/source/Silver_bromide) | bgcolor="#FFCCCC" | [I](/source/silver_iodide) | bgcolor="#99CCFF" | [S](/source/Silver_perchlorate) | bgcolor="#FFCCCC" | [I](/source/Silver_oxide) | bgcolor="#FFCCCC" | [I](/source/Silver_hydroxide) | bgcolor="#FFCCCC" | [I](/source/Silver_sulfide) | bgcolor="#CCCCFF" | [sS](/source/Silver_sulfate) | bgcolor="#99CCFF" | [S](/source/Silver_nitrate) | bgcolor="#FFCCCC" | [I](/source/Silver_azide) | bgcolor="#FFCCCC" | [I](/source/Silver_phosphate) | bgcolor="#FFCCCC" | [I](/source/Silver_carbonate) | bgcolor="#FFCCCC" | [I](/source/Silver_cyanide) | bgcolor="#FFCCCC" | [I](/source/Silver_thiocyanate) | bgcolor="#CCCCFF" | [sS](/source/Silver_acetate) | bgcolor="#FFCCCC" | [I](/source/Silver_oxalate) |- align="center" ! [Mercury](/source/Mercury_(element))(I) {{chem|Hg|2|2+}} | bgcolor="#CCCCCC" | [R](/source/Mercury(I)_fluoride) | bgcolor="#FFCCCC" | [I](/source/Mercury(I)_chloride) | bgcolor="#FFCCCC" | [I](/source/Mercury(I)_bromide) | bgcolor="#FFCCCC" | [I](/source/Mercury(I)_iodide) | bgcolor="#99CCFF" | [S](/source/Mercury(I)_perchlorate){{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](/source/Mercury(I)_oxide) | ? | [?](/source/Mercury(I)_sulfide) | bgcolor="#CCCCFF" | [sS](/source/Mercury(I)_sulfate) | bgcolor="#99CCFF" | [S](/source/Mercury(I)_nitrate){{efn|name=MercurousSlowReact|group=lower-alpha|Slowly decomposes in water.}} | bgcolor="#FFCCCC" | [I](/source/Mercury(I)_azide) | ? | bgcolor="#FFCCCC" | [I](/source/Mercury(I)_carbonate) | bgcolor="#FFCCCC" | [I](/source/Mercury(I)_cyanide) | ? | bgcolor="#99CCFF" | [S](/source/Mercury(I)_acetate){{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="5.56%" |   ! width="5.56%" | [Fluoride](/source/Fluoride)
F− ! width="5.56%" | [Chloride](/source/Chloride)
Cl− ! width="5.56%" | [Bromide](/source/Bromide)
Br− ! width="5.56%" | [Iodide](/source/Iodide)
I− ! width="5.56%" | [Perchlorate](/source/Perchlorate)
{{chem|ClO|4|−}} ! width="5.56%" | [Oxide](/source/Oxide)
O2− ! width="5.56%" | [Hydroxide](/source/Hydroxide)
OH− ! width="5.56%" | [Sulfide](/source/Sulfide)
S2− ! width="5.56%" | [Sulfate](/source/Sulfate)
{{chem|SO|4|2−}} ! width="5.56%" | [Nitrate](/source/Nitrate)
{{chem|NO|3|−}}{{efn|name=AlwaysSolubleK}} ! width="5.56%" | [Azide](/source/Azide)
{{chem|N|3|−}} ! width="5.56%" | [Phosphate](/source/Phosphate)
{{chem|PO|4|3−}} ! width="5.56%" | [Carbonate](/source/Carbonate)
{{chem|CO|3|2−}}{{efn|name=AlwaysSolubleK}} ! width="5.56%" | [Cyanide](/source/Cyanide)
CN− ! width="5.56%" | [Thiocyanate](/source/Thiocyanate)
SCN− ! width="5.56%" | [Acetate](/source/Acetate)
{{chem|C|2|H|3|O|2|−}} ! width="5.56%" | [Oxalate](/source/Oxalate)
{{chem|C|2|O|4|2−}} |} ==See also== *[Solubility rules](/source/Solubility_rules) == Notes == {{reflist|group=lower-alpha}} == References == {{reflist}} {{Chemical solutions}} Category:Solutions --- Adapted from the Wikipedia article [Solubility chart](https://en.wikipedia.org/wiki/Solubility_chart) by Wikipedia contributors ([contributor history](https://en.wikipedia.org/wiki/Solubility_chart?action=history)). Available under [Creative Commons Attribution-ShareAlike 4.0 International](https://creativecommons.org/licenses/by-sa/4.0/). Changes may have been made.