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|Section2= |Section3= |Section4= |Section7= |Section8= }} Barium chloride is the inorganic compound with the formula BaCl2. It is one of the most common water-soluble salts of barium. Like other barium salts, it is toxic and imparts a yellow-green coloration to a flame. It is also hygroscopic. ==Structure and properties== BaCl2 crystallizes in two forms (polymorphs). One form has the cubic fluorite (CaF2) structure and the other the orthorhombic cotunnite (PbCl2) structure. Both polymorphs accommodate the preference of the large Ba2+ ion for coordination numbers greater than six.〔Wells, A. F. (1984) ''Structural Inorganic Chemistry'', Oxford: Clarendon Press. ISBN 0-19-855370-6.〕 The coordination of Ba2+ is 8 in the fluorite structure and 9 in the cotunnite structure.〔 〕 When cotunnite-structure BaCl2 is subjected to pressures of 7–10 GPa, it transforms to a third structure, a monoclinic post-cotunnite phase. The coordination number of Ba2+ increases from 9 to 10. In aqueous solution BaCl2 behaves as a simple salt; in water it is a 1:2 electrolyte and the solution exhibits a neutral pH. Its solutions react with sulfate ion to produce a thick white precipitate of barium sulfate. :Ba2+(aq) + SO42−(aq) → BaSO4(s) Oxalate effects a similar reaction: :Ba2+(aq) + C2O42−(aq) → BaC2O4(s) When it is mixed with sodium hydroxide, it gives the dihydroxide, which is moderately soluble in water. 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Barium chloride」の詳細全文を読む スポンサード リンク
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