Solubility chart solubility chart list of ions and how , when mixed with other ions, they can become precipitates or remain aqueous.shows the solubility of multiple independent and various compounds , in water, at a pressure of 1 atm and at room temperature . 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, 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 .boiling point to fully dissolve.water-soluble . In a base, dichromates convert into chromates and some of the chromates are insoluble in water. Fluoride− Chloride− Bromide− Iodide− Carbonate3 2− Chlorate3 − Hydroxide− Cyanide− Cyanate− Thiocyanate− Nitrate3 − Oxide2− Phosphate4 3− Sulfate4 2− Dichromate2 O7 2− Lithium+ sS S S S sS S S S ? S S R I S S Sodium+ S S S S S S S S S S S R S S S Potassium+ S S S S S S S S S S S R S S S Ammonium4 + S S S S S S S S ? S S ? S S S Beryllium2+ S S S R I ? ? ? ? ? S R ? S ? Magnesium2+ sS S S S I S I ? ? ? S I I S S Calcium2+ I S S S I S sS S ? ? S R I sS S Strontium2+ sS S S S I S S ? ? ? S R ? I ? Barium2+ sS S S S I S S S ? ? S R I I ? Zinc2+ sS S S S I S I I ? ? S I I S S Iron2+ S S S S I S I ? ? ? S I I S S Copper2+ sS S S ? I S I ? ? I S I I S S Aluminium3+ S S S S ? S I ? ? ? S I I S S Iron3+ X S S ? X S I ? ? ? S I I sS S Lead2+ sS sS sS I I S I ? ? sS S I I I ? Silver+ S I I I I S sS I I sS S sS I sS S Fluoride− Chloride− Bromide− Iodide− Carbonate3 2− Chlorate3 − Hydroxide− Cyanide− Cyanate− Thiocyanate− Nitrate3 − Oxide2− Phosphate4 3− Sulfate4 2− Dichromate2 O7 2−
S soluble I insoluble sS slightly soluble X other R reacts with water ? unavailable
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