Barium chloride 1055399 222098973 2008-06-27T15:34:40Z Ecopetition 3658153 /* Safety */ BaCl2 is highly toxic {{Chembox new | Name = Barium chloride | ImageFile = Barium chloride.jpg | ImageSize = 200px | ImageName = Barium chloride | Section1 = {{Chembox Identifiers | CASNo = 10361-37-2 }} | Section2 = {{Chembox Properties | Formula = [[Barium|Ba]][[Chlorine|Cl]]<sub>2</sub> (anhydrous)<br /> BaCl<sub>2</sub>&middot;2H<sub>2</sub>O | MolarMass = 208.2324 g/mol | Appearance = White solid | Density = 3.856&nbsp;g/cm<sup>3</sup>,&nbsp;solid | Solubility = 37.5 g/100 ml (26°C) | MeltingPt = 962 °C | BoilingPt = 1560 °C }} | Section3 = {{Chembox Structure | Coordination = 7-9 | CrystalStruct = [[monoclinic]] or [[orthorhombic]] }} | Section4 = {{Chembox Thermochemistry | DeltaHf = &minus;858.56 kJ/mol }} | Section7 = {{Chembox Hazards | EUClass = Toxic ('''T''') | RPhrases = {{R20}}, {{R25}} | SPhrases = {{S1/2}}, {{S45}} | FlashPt = Non-flammable }} | Section8 = {{Chembox Related | OtherAnions = [[Barium fluoride]]<br />[[Barium bromide]]<br />[[Barium iodide]] | OtherCations = [[Calcium chloride]]<br /> [[Strontium chloride]]<br /> [[Lead chloride]] }} }} '''[[Barium]] [[chloride]]''' is the ionic [[chemical compound]] with the [[chemical formula|formula]] BaCl<sub>2</sub>. It is one of the most important 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== BaCl<sub>2</sub> crystallizes in both the [[fluorite]] and [[lead chloride]] motifs, both of which accommodate the preference of the large Ba<sup>2+</sup> ion for coordination numbers greater than six.<ref>Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.</ref> In aqueous solution BaCl<sub>2</sub> behaves as a simple [[salt]]; in water it is a 1:2 electrolyte and the solution exhibits a neutral [[pH]]. Barium chloride reacts with [[sulfate]] [[ion]] to produce a thick white [[precipitate]] of [[barium sulfate]]. :BaCl<sub>2</sub>([[aqueous|aq]]) + SO<sub>4</sub><sup>2-</sup> → BaSO<sub>4</sub>([[solid|s]]) + 2 [[chloride|Cl<sup>-</sup>]](aq) [[Oxalate]] effects a similar reaction: :BaCl<sub>2</sub>(aq) + [[sodium oxalate|Na<sub>2</sub>C<sub>2</sub>O<sub>4</sub>]](aq) → Ba<sub></sub>C<sub>2</sub>O<sub>4</sub> (s) + 2 [[sodium chloride|NaCl]](aq) ==Preparation== Although inexpensively available, barium chloride can be prepared from [[barium hydroxide]] or [[barium carbonate]], the latter 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]])<sup>[4]</sup>: :BaSO<sub>4</sub> + 4 [[carbon|C]] → BaS + 4 [[carbon monoxide|CO]] This first step requires high temperatures. :BaS + [[calcium chloride|CaCl<sub>2</sub>]] → BaCl<sub>2</sub> + [[calcium sulfide|CaS]] The second step reqiures [[melting|fusion]] of the reactants. The BaCl<sub>2</sub> can then be leached out from the mixture with [[water]]. ==Uses== As a cheap, 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. BaCl<sub>2</sub> is also used in [[fireworks]] to give a bright green color. However, its toxicity limits its applicability. Barium Chloride is also used (with Hydrochloric acid) as a test for sulfates. When these two chemicals are mixed with a sulfate salt, a white precipitate forms, which is barium sulfate. ==Safety== Barium chloride, along with other water-soluble barium salts, is highly toxic. [[Sodium sulfate]] is a potential antidote because it forms the insoluble solid BaSO<sub>4</sub>. ==References== <references/> # Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford: Butterworth-Heinemann. ISBN 0-7506-3365-4. # ''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990. # ''The Merck Index'', 7th edition, Merck & Co., Rahway, New Jersey, 1960. # H. Nechamkin, ''The Chemistry of the Element'', McGraw-Hill, New York, 1968. ==External links== * [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc06/icsc0614.htm International Chemical Safety Card 0614]. (''anhydrous'') * [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc06/icsc0615.htm International Chemical Safety Card 0615]. (''dihydrate'') * [http://www.cdc.gov/niosh/npg/npgd0045.html NIOSH Pocket Guide to Chemical Hazards]. * [http://ecb.jrc.it/ European Chemicals Bureau]. * [http://www.solvayvishnubarium.com/products/bariumchloride/0,,4872-2-0,00.htm Barium chloride's use in industry]. [[Category:Chlorides]] [[Category:Metal halides]] [[Category:Barium compounds]] [[Category:Inorganic compounds]] [[Category:Pyrotechnic colorants]] [[ar:كلوريد باريوم]] [[de:Bariumchlorid]] [[fr:Chlorure de baryum]] [[it:Cloruro di bario]] [[lv:Bārija hlorīds]] [[hu:Bárium-klorid]] [[ja:塩化バリウム]] [[pl:Chlorek baru]] [[simple:Barium chloride]] [[sv:Bariumklorid]] [[th:แบเรียมคลอไรด์]] [[uk:Хлорид барію]] [[zh:氯化钡]]