barium chloride dihydrate |
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Item : cas 10361-37-2 |
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Details :Barium Chloride Dihydrate
CAS No.:10361-37-2 Molecular formula BaCl2.2H2O244
molecular weight:.277 UN NO. 1564 IMO Class: 6.1 Character:Colourless,flat rhombus crystal,usually with two crystal water.Specific gravity:3.097(24/4 ).Dissllving point:962 .Boiling point:1560 poisonous.Wash in water whin getting in on the skin.After poisoning,take sodium sulphate or magnesium sulphate.
Use:As a raw material for producing bariumn salts,such as barium hydroxide barium nitrate and barium carbonate etc.Widely used in papermaking dyestuff rubber plastic ceramics iol refining and petrochemistry and so on.Also used to heat-treat the metals and remove sulphate in the salt water in chlorine-alkaki industry.
Storage and transportation:Keep dry and prevent damp.
Packing:Packed in polypropylene bag,lined with polyethylene bag,50kgs or 25kgs/bag net. Barium chlorideFrom Wikipedia, the free encyclopedia
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.
[edit] Structure and propertiesBaCl2 crystallizes in two forms (polymorphs). One form resembles fluorite and the other lead chloride motifs. Both polymorphs accommodate the preference of the large Ba2+ ion for coordination numbers greater than six.[2] 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.
Oxalate effects a similar reaction:
When it is mixed with sodium hydroxide, it gives the dihydroxide, which is moderately soluble in water. [edit] PreparationBarium chloride can be prepared from barium hydroxide or barium carbonate, with barium carbonate being found naturally as the mineral witherite. These basic salts react with hydrochloric acid to give hydrated barium chloride. On an industrial scale, it is prepared via a two step process from barite (barium sulfate):[3] This first step requires high temperatures. The second step requires fusion of the reactants. The BaCl2 can then be leached out from the mixture with water. From water solutions of barium chloride, the dihydrate can be crystallized as white crystals: BaCl2·2H2O [edit] UsesAs an inexpensive, soluble salt of barium, barium chloride finds wide application in the laboratory. It is commonly used as a test for sulfate ion (see chemical properties above). In industry, barium chloride is mainly used in the purification of brine solution in caustic chlorine plants and also in the manufacture of heat treatment salts, case hardening of steel, in the manufacture of pigments, and in the manufacture of other barium salts. BaCl2 is also used in fireworks to give a bright green color. However, its toxicity limits its applicability. [edit] SafetyBarium chloride, along with other water-soluble barium salts, is highly toxic.[4] Sodium sulfate and magnesium sulfate are potential antidotes because they form the insoluble solid barium sulfate BaSO4, which is nontoxic. [edit] References
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