Summary
A solubility chart is a chart with a list of ions and how, when mixed with other ions, they can become precipitates or remain aqueous.
The following chart shows the solubility of multiple independent and various compounds, in water, at a pressure of 1 atm and at room temperature (approx. 25 °C (298.15 K)). Any box that reads "soluble" results in an aqueous product in which no precipitate has formed, while "slightly soluble" and "insoluble" markings mean that there is a precipitate that will form (usually, this is a solid); however, "slightly soluble" compounds such as calcium sulfate may require heat to form its precipitate. Boxes marked "other" can mean that many different states of products can result. For more detailed information of the exact solubility of the compounds, see the solubility table.
The chemicals have to be exposed to their boiling point to fully dissolve.
Note: All the dichromates are water-soluble. In a base, dichromates convert into chromates and some of the chromates are insoluble in water.
| Fluoride F− |
Chloride Cl− |
Bromide Br− |
Iodide I− |
Oxide O2− |
Sulfide S2− |
Selenide Se2− |
Nitride N3− |
Hydroxide OH− |
Cyanide CN− |
Thiocyanate SCN− |
Nitrate NO− 3 |
Acetate C 2H 3O− 2 |
Carbonate CO2− 3 |
Sulfate SO2− 4 |
Oxalate C 2O2− 4 |
Phosphate PO3− 4 | |
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| Ammonium NH+ 4[a] |
S | S | S | S | S* | S | R[1] | S | S | S | S | S | S | S | S | S | S |
| Hydrogen H+ |
S | S | S | S | S | S | sS | S | S | S | S | S | S | S | S | S | S |
| Lithium Li+ |
sS | S | S | S | R | R | R | R | S | S | S | S | S | S | S | S | sS |
| Sodium Na+ |
S | S | S | S | R | R | R | R | S | S | S | S | S | S | S | S | S |
| Potassium K+ |
S | S | S | S | R | R | R | R | S | S | S | S | S | S | S | S | S |
| Rubidium Rb+ |
S | S | S | S | R | R | R | ? | S | S | S | S | S | S | S | I | I |
| Caesium Cs+ |
S | S | S | S | R | R | R | ? | S | S | S | S | S | S | S | I | S |
| Beryllium Be2+ |
S | S | S | R | I | R | S | R | I | S | S | S | S | I | S | I | S |
| Magnesium Mg2+ |
sS | S | S | S | I | R | R | R | I | S | S | S | S | I | S | sS | I |
| Calcium Ca2+ |
I | S | S | S | R | R | R | R | sS | S | S | S | S | I | sS | sS | I |
| Strontium Sr2+ |
sS | S | S | S | R | sS | I | R | S | S | S | S | S | I | I | I | sS |
| Barium Ba2+ |
sS | S | S | S | R | S | R | S | S | S | S | S | S | sS | I | I | I[2] |
| Boron B3+ |
R | S | R | S | S | R | R[3] | I | S | S | S | X | S | ? | S | ? | I |
| Aluminium Al3+ |
S | S | S | S (partial electrolysis) | I | R | R | I | I | R | S | S | S | R | S | I | I |
| Gallium Ga3+ |
sS | S | S | R | I | S | R | I | I | S | S | S | S | R | sS | ? | I |
| Manganese(II) Mn2+ |
S | S | S | S | I | I | I | I | I | S | I | S | S | I | S | I | I |
| Iron(II) Fe2+ |
S | S | S | S | I | I | I | I | I | S | S | S | S | I | S | I | I |
| Cobalt(II) Co2+ |
S | S | S | S | I | I | I | I | I | I | S | S | S | I | S | I | I |
| Nickel(II) Ni2+ |
S | S | S | S | I | I | I | I | I | I | S | S | S | I | S | I | I |
| Copper(II) Cu2+ |
sS | S | S | X | I | I | I | I | I | I | I | S | S | R | S | I | I |
| Zinc Zn2+ |
sS | S | S | S | I | I | I | R | I | I | S | S | S | I | S | I | I |
| Tin(II) Sn2+ |
S | S | S | S | I | I | I | I | I | S | sS | S | R | I | S | sS | I |
| Mercury(II) Hg2+ |
R | S | S | I | I | I | I | R | I | S | sS | S | S | I | R | I | I |
| Lead(II) Pb2+ |
sS | S | sS | sS | I | I | I | ? | I | sS | sS | S | S | I | I | sS | I |
| Vanadium(III) V3+ |
I | S | S | S | I | I | ? | I | ? | ? | S | S | ? | ? | S | ? | I |
| Chromium(III) Cr3+ |
I | sS | sS | S | I | I | I | I | I | S | S | S | S | I | I | ? | I |
| Iron(III) Fe3+ |
S[b] | S | S | R | I | sS | ? | I | I | S | S | S | S | R[4] | S | sS | I |
| Titanium(IV) Ti4+ |
R | R | R | R | I | I | I | ? | I[5] | ? | ? | S | R | ? | R[5] | I | I |
| Silver Ag+ |
S | I | I | I | I | I | I | sS | I | I | sS | S | S | I | sS | I | I |
| Gold Au3+ |
I | S | sS | I | I | I | ? | I | I | S | ? | S | S | I | S | ? | ? |
| Fluoride F− |
Chloride Cl− |
Bromide Br− |
Iodide I− |
Oxide O2− |
Sulfide S2− |
Selenide Se2− |
Nitride N3− |
Hydroxide OH− |
Cyanide CN− |
Thiocyanate SCN− |
Nitrate NO− 3[a] |
Acetate C 2H 3O− 2 |
Carbonate CO2− 3[a] |
Sulfate SO2− 4 |
Oxalate C 2O2− 4 |
Phosphate PO3− 4 |
- Note: "Ammonium oxide" does not exist. However, its theoretical molecular formula (NH+
4)2O2− accurately represents that of aqueous ammonia.
| S | soluble | 0.01 ~ 100 mL (of water needed to dissolve 1 gram of solute) |
| sS | slightly soluble | 100 mL ~ 10 L |
| I | insoluble | 10 L and up |
| X | other | N/A |
| R | reacts with water | N/A |
| ? | unavailable | N/A |
See alsoEdit
NotesEdit
- ^ a b c Compounds that include ammonium (NH+
4), chlorate (ClO−
3), or nitrate (NO−
3) are soluble without exceptions. Compounds that include carbonate (CO2−
3) are insoluble, unless the compound includes group 1 elements or ammonium.[6] - ^ Anhydrous FeF3 is slightly soluble in water, FeF3·3H2O is much more soluble in water.
ReferencesEdit
- ^ "Ammonium Selenide", JACS, 1898-02-26
- ^ Hazen, Jeffery L.; Cleary, David A. (July 2, 2014). "Yielding Unexpected Results: Precipitation of Ba3(PO4)2 and Implications for Teaching Solubility Principles in the General Chemistry Curriculum". Journal of Chemical Education. 91 (8): 1261–1263. doi:10.1021/ed400741k.
- ^ "Boron Selenide". American Elements. January 5, 2021.
- ^ "Iron (III) Carbonate Formula": 1.
{{cite journal}}: Cite journal requires|journal=(help) - ^ a b Frederick Pearson Treadwell (1916). Qualitative analysis. J.Wiley & sons, Incorporated. p. 538. Retrieved 26 March 2021.
- ^ "Solubility Table". intro.chem.okstate.edu.