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Barium carbonate is the inorganic compound with the formula BaCO 3. Like most alkaline earth metal carbonates, it is a white salt that is poorly soluble in water. It occurs as the mineral known as witherite. In a commercial sense, it is one of the most important barium compounds. [5]
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.
Barium bromide – BaBr 2; Barium carbonate – BaCO 3 ... Ceric ammonium nitrate – (NH 4) 2 Ce(NO 3) 6; ... Water - H 2 O [204] He
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.
Barium chloride: Solid BaCl 2: −858.6 Barium carbonate: Solid BaCO 3: −1216 Barium hydroxide: Solid Ba(OH) 2: −944.7 Barium oxide: Solid BaO −548.1 Barium sulfate: Solid BaSO 4: −1473.3 Beryllium: Solid Be 0 Beryllium hydroxide: Solid Be(OH) 2: −903 Beryllium oxide: Solid BeO −609.4 Boron trichloride: Solid BCl 3: −402.96 ...
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
Barium hydroxide is used in analytical chemistry for the titration of weak acids, particularly organic acids. Its aqueous solution, if clear, is guaranteed to be free of carbonate, unlike those of sodium hydroxide and potassium hydroxide, as barium carbonate is insoluble in water.
Note that the especially high molar values, as for paraffin, gasoline, water and ammonia, result from calculating specific heats in terms of moles of molecules. If specific heat is expressed per mole of atoms for these substances, none of the constant-volume values exceed, to any large extent, the theoretical Dulong–Petit limit of 25 J⋅mol ...