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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]
BaSi 2: barium silicide: 1304-40-1 BaSi 2 O 5: barium disilicate: 12650-28-1 BaSnO 3: barium stannate: 12009-18-6 BaTeO 3: barium tellurite: 58440-17-8 BaTeO 4 ·3H 2 O: barium tellurate trihydrate: 28557-54-2 BaTiO 3: barium titanate barium metatitanate: 12047-27-7 BaU 2 O 7: barium uranium oxide: 10380-31-1 BaWO 4: barium tungstate: 7787-42-0 ...
BaSi 2: barium silicide: 1304–40–1 BaSi 2 O 5: barium disilicate: 12650–28–1 BaSnO 3: barium stannate: 12009–18–6 BaTiO 3: barium titanate: 12047–27–7 Ba(VO 3) 2: barium vanadate: 22652–39–7 BaWO 4: barium tungstate: 7787–42–0 BaZrO 3: barium zirconate: 12009–21–1 Ba 2 P 2 O 7: barium pyrophosphate: 13466–21–2 Ba ...
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.
This is also called the Wohl–Ziegler reaction. [8] [9] The carbon tetrachloride must be maintained anhydrous throughout the reaction, as the presence of water may likely hydrolyze the desired product. [10] Barium carbonate is often added to maintain anhydrous and acid-free conditions.
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).
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
Barium bromide can be prepared by treating barium sulfide or barium carbonate with hydrobromic acid: BaS + 2 HBr → BaBr 2 + H 2 S BaCO 3 + 2 HBr → BaBr 2 + CO 2 + H 2 O. Barium bromide crystallizes from concentrated aqueous solution in its dihydrate, BaBr 2 ·2H 2 O. Heating this dihydrate to 120 °C gives the anhydrous salt. [6]