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>·2H<sub>2</sub>O
| MolarMass = 208.2324 g/mol
| Appearance = White solid
| Density = 3.856 g/cm<sup>3</sup>, 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 = −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]]