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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]
Iron(III) nitrate – Fe(NO 3) 3 (H 2 O) 9; Iron(III) sulfate – Fe 2 (SO 4) 3; Iron(III) thiocyanate – Fe(SCN) 3; Iron(II,III) oxide – Fe 3 O 4; Iron ferrocyanide – Fe 7 (CN) 18; Prussian blue (Iron(III) hexacyanoferrate(II)) – Fe 4 [Fe(CN) 6] 3; Ammonium iron(II) sulfate – (NH 4) 2 Fe(SO 4) 2; Iron(II) bromide – FeBr 2; Iron(III ...
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 ...
Barium salts are typically white when solid and colorless when dissolved. [14] They are denser than the strontium or calcium analogs, except for the halides (see table; zinc is given for comparison). Barium hydroxide ("baryta") was known to alchemists, who produced it by heating
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).
It is isoelectronic with nitric acid HNO 3. The bicarbonate ion carries a negative one formal charge and is an amphiprotic species which has both acidic and basic properties. It is both the conjugate base of carbonic acid H 2 CO 3; and the conjugate acid of CO 2− 3, the carbonate ion, as shown by these equilibrium reactions: CO 2− 3 + 2 H 2 ...
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure.
Barium acetate is generally produced by the reaction of acetic acid with barium carbonate: [2] BaCO 3 + 2 CH 3 COOH → (CH 3 COO) 2 Ba + CO 2 + H 2 O. The reaction is performed in solution and the barium acetate crystalizes out at temperatures above 41 °C. Between 25 and 40 °C, the monohydrate version crystalizes. Alternatively, barium ...