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The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "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.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/(100 mL)), unless shown otherwise. The substances are listed in alphabetical order.
Silver nitrite is much less soluble in water than silver nitrate, and a solution of silver nitrate will readily precipitate silver nitrite upon addition of sodium nitrite: AgNO 3 (aq) + NaNO 2 (s) → NaNO 3 (aq) + AgNO 2 (precipitate) Alternatively, it can be produced by the reaction between silver sulfate and barium nitrite.
Silver sulfate precipitates as a solid when an aqueous solution of silver nitrate is treated with sulfuric acid: . 2 AgNO 3 + H 2 SO 4 → Ag 2 SO 4 + 2 HNO 3. It is purified by recrystallization from concentrated sulfuric acid, a step that expels traces of nitrate. [7]
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Silver nitrate is currently unregulated in water sources by the United States Environmental Protection Agency. However, if more than 1 gram of silver is accumulated in the body, a condition called argyria may develop. Argyria is a permanent cosmetic condition in which the skin and internal organs turn a blue-gray color.
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The solubility of a specific solute in a specific solvent is generally expressed as the concentration of a saturated solution of the two. [1] Any of the several ways of expressing concentration of solutions can be used, such as the mass, volume, or amount in moles of the solute for a specific mass, volume, or mole amount of the solvent or of the solution.