Cobalt ( II ) chloride - wikipedia Cobalt ( II ) chloride `` CoCl2 '' redirects here. For the compound COCl, see Phosgene. Cobalt ( II ) chloride Anhydrous Hexahydrate Structure of anhydrous compound Structure of hexahydrate Names IUPAC name Cobalt ( II ) chloride Other names Cobaltous chloride Cobalt dichloride Muriate of cobalt Identifiers CAS Number 7646 - 79 - 9 16544 - 92 - 6 ( dihydrate ) 7791 - 13 - 1 ( hexahydrate ) 3D model ( JSmol ) Interactive image ChEBI CHEBI : 35696 ChemSpider 22708 ECHA InfoCard 100.028. 718 EC Number 231 - 589 - 4 PubChem CID 3032536 RTECS number GF9800000 UNII EVS87XF13W UN number 3288 InChI InChI = 1S / 2ClH.Co/h2 * 1H ; / q ; ; + 2 / p - 2 Key : GVPFVAHMJGGAJG - UHFFFAOYSA - L InChI = 1 / 2ClH.Co/h2 * 1H ; / q ; ; + 2 / p - 2 Key : GVPFVAHMJGGAJG - NUQVWONBAU SMILES Cl ( Co ) Cl Properties Chemical formula CoCl Molar mass 129.839 g / mol ( anhydrous ) 165.87 g / mol ( dihydrate ) 237.93 g / mol ( hexahydrate ) Appearance blue crystals ( anhydrous ) violet - blue ( dihydrate ) rose red crystals ( hexahydrate ) Density 3.356 g / cm ( anhydrous ) 2.477 g / cm ( dihydrate ) 1.924 g / cm ( hexahydrate ) Melting point 735 ° C ( 1,355 ° F ; 1,008 K ) ( anhydrous ) 140 ° C ( monohydrate ) 100 ° C ( dihydrate ) 86 ° C ( hexahydrate ) Boiling point 1,049 ° C ( 1,920 ° F ; 1,322 K ) Solubility in water 43.6 g / 100 mL ( 0 ° C ) 45 g / 100 mL ( 7 ° C ) 52.9 g / 100 mL ( 20 ° C ) 105 g / 100 mL ( 96 ° C ) Solubility 38.5 g / 100 mL ( methanol ) 8.6 g / 100 mL ( acetone ) soluble in ethanol, pyridine, glycerol Magnetic susceptibility ( χ ) + 12,660 10 cm / mol Structure Crystal structure CdCl structure Coordination geometry hexagonal ( anhydrous ) monoclinic ( dihydrate ) Octahedral ( hexahydrate ) Hazards Safety data sheet ICSC 0783 EU classification ( DSD ) ( outdated ) Toxic ( T ) Carc. Cat. 2 Dangerous for the environment ( N ) R - phrases ( outdated ) R49, R60, R22, R42 / 43, R68, R50 / 53 S - phrases ( outdated ) S53, S45, S60, S61 NFPA 704 0 0 Flash point Non-flammable Lethal dose or concentration ( LD, LC ) : LD ( median dose ) 80 mg / kg ( rat, oral ) Related compounds Other anions Cobalt ( II ) fluoride Cobalt ( II ) bromide Cobalt ( II ) iodide Other cations Rhodium ( III ) chloride Iridium ( III ) chloride Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). N verify ( what is ? ) Infobox references Cobalt ( II ) chloride is an inorganic compound of cobalt and chlorine, with the formula CoCl. It is usually supplied as the hexahydrate CoCl 6H O, which is one of the most commonly used cobalt compounds in the lab. The hexahydrate is purple, whereas the anhydrous form is sky blue. Because of the ease of the hydration / dehydration reaction, and the resulting color change, cobalt chloride is used as an indicator for water in desiccants. Niche uses of cobalt chloride include its role in organic synthesis and electroplating objects with cobalt metal. Cobalt chloride has been classified as a substance of very high concern by the European Chemicals Agency as it is a suspected carcinogen. Contents 1 Properties 2 Preparation 3 Reactions 3.1 Co ( III ) derivatives 3.2 Instability of CoCl 4 Safety 5 Other uses 6 References 7 External links Properties Aqueous solutions of both CoCl and the hydrate contain the species ( Co ( H O ) ). They also contain chloride ions. Solid CoCl 6H O consists of the molecule trans - ( CoCl ( H O ) ) and two molecules of water of crystallization. This species dissolves readily in water and alcohol. Concentrated aqueous solutions are red at room temperature but become blue at higher temperatures. CoCl 6H O is deliquescent, and the anhydrous salt CoCl is hygroscopic. Preparation Hydrated cobalt chloride is prepared from cobalt ( II ) hydroxide or cobalt ( II ) carbonate and hydrochloric acid : CoCO + 2 HCl + 5 H O → Co ( H O ) Cl + CO Upon heating, the hexahydrate dehydrates. Dehydration can also be effected with trimethylsilyl chloride : CoCl 6H O + 12 Me SiCl → CoCl + 6 ( Me Si ) O + 12 HCl Reactions Generally, aqueous solutions of cobalt ( II ) chlorides behave like other cobalt ( II ) salts since these solutions consist of the ( Co ( H O ) ) ion regardless of the anion. Such solutions give a precipitate of CoS upon treatment with H S. CoCl 6H O and CoCl are weak Lewis acids. The adducts are usually either octahedral or tetrahedral. With pyridine ( C 5H 5N ), one obtains the octahedral complex : CoCl 6H O + 4 C H N → CoCl ( C H N ) + 6 H O With triphenylphosphine ( P ( C 6H 5 ) 3 ), a tetrahedral complex results : CoCl 6H O + 2 P ( C H ) → CoCl ( P ( C H ) ) + 6 H O Salts of the anionic complex CoCl can be prepared using tetraethylammonium chloride : CoCl + 2 ( ( C H ) N ) Cl → ( ( C H ) N ) ) ( CoCl ) The ( CoCl ) ion is the blue ion that forms upon addition of hydrochloric acid to aqueous solutions of hydrated cobalt chloride, which are pink. The structure of a cobalt ( IV ) coordination complex with the norbornyl anion In the laboratory, cobalt ( II ) chloride serves as a common precursor to other cobalt compounds. Reaction of the anhydrous compound with sodium cyclopentadienide gives cobaltocene. This 19 - electron species is a good reducing agent, being readily oxidised to the yellow 18 - electron cobaltacenium cation. Reaction of 1 - norbonyllithium with the CoCl THF in pentane produces the brown, thermally stable cobalt ( IV ) tetralkyl -- a rare example of a stable transition metal / saturated alkane compound, different products are obtained in other solvents. Co ( III ) derivatives In the presence of ammonia or amines, cobalt ( II ) is readily oxidised by atmospheric oxygen to give a variety of cobalt ( III ) complexes. For example, the presence of ammonia triggers the oxidation of cobalt ( II ) chloride to hexamminecobalt ( III ) chloride : 4 CoCl 6H O + 4 NH Cl + 20 NH + O → 4 ( Co ( NH ) ) Cl + 26 H O The reaction is often performed in the presence of charcoal as a catalyst, or hydrogen peroxide is employed in place of air. Other highly basic ligands including carbonate, acetylacetonate, and oxalate induce the formation of Co ( III ) derivatives. Simple carboxylates and halides do not. Unlike Co ( II ) complexes, Co ( III ) complexes are very slow to exchange ligands, so they are said to be kinetically inert. The German chemist Alfred Werner was awarded the Nobel prize in 1913 for his studies on a series of these cobalt ( III ) compounds, work that led to an understanding of the structures of such coordination compounds. Instability of CoCl Anhydrous cobalt ( II ) chloride The existence of cobalt ( III ) chloride, CoCl, is disputed, although this compound is listed in some compendia. According to Greenwood and Earnshaw, the only stable binary compounds of cobalt and the halogens, excluding CoF, are the dihalides. Stated differently, CoCl is unreactive toward Cl. The stability of Co ( III ) in solution is considerably increased in the presence of ligands of greater Lewis basicity than chloride, such as amines. Safety Patch test In 2005 -- 06, cobalt chloride was the eighth-most - prevalent allergen in patch tests ( 8.4 % ). Other uses Invisible ink Cobalt chloride is an established chemical inducer of hypoxia - like responses such as erythropoiesis. Cobalt supplementation is not banned and therefore would not be detected by current anti-doping testing. Cobalt chloride is a banned substance under the Australian Thoroughbred Racing References Jump up ^ http://www.chemindustry.com/chemicals/0519906.html. ^ Jump up to : Greenwood, Norman N. ; Earnshaw, Alan ( 1997 ). Chemistry of the Elements ( 2nd ed. ). Butterworth - Heinemann. ISBN 0 - 08 - 037941 - 9. Jump up ^ Wells, A.F. ( 1984 ), Structural Inorganic Chemistry ( 5th ed. ), Oxford : Clarendon Press, ISBN 0 - 19 - 855370 - 6 Jump up ^ The Merck Index, 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960. Jump up ^ John Dallas Donaldson, Detmar Beyersmann, `` Cobalt and Cobalt Compounds '' in Ullmann 's Encyclopedia of Industrial Chemistry, Wiley - VCH, Weinheim, 2005. doi : 10.1002 / 14356007. a07_281. pub2 Jump up ^ Philip Boudjouk, Jeung - Ho So ( 1992 ). `` Solvated and Unsolvated Anhydrous Metal Chlorides from Metal Chloride Hydrates ''. Inorg. Synth. 29 : 108 -- 111. doi : 10.1002 / 9780470132609. ch26. CS1 maint : Uses authors parameter ( link ) Jump up ^ Gill, N.S. & Taylor, F.B. ( 1967 ). `` Tetrahalo Complexes of Dipositive Metals in the First Transition Series ''. Inorg. Synth. 9 : 136 -- 142. doi : 10.1002 / 9780470132401. ch37. Jump up ^ Barton K. Bower & Howard G. Tennent ( 1972 ). `` Transition metal bicyclo ( 2.2. 1 ) hept - 1 - yls ''. J. Am. Chem. Soc. 94 ( 7 ) : 2512 -- 2514. doi : 10.1021 / ja00762a056. Jump up ^ Erin K. Byrne ; Darrin S. Richeson & Klaus H. Theopold ( 1986 ). `` Tetrakis ( 1 - norbornyl ) cobalt, a low spin tetrahedral complex of a first row transition metal ''. J. Chem. Soc., Chem. Commun. ( 19 ) : 1491 -- 1492. doi : 10.1039 / C39860001491. Jump up ^ Erin K. Byrne ; Klaus H. Theopold ( 1989 ). `` Synthesis, characterization, and electron - transfer reactivity of norbornyl complexes of cobalt in unusually high oxidation states ''. J. Am. Chem. Soc. 111 ( 11 ) : 3887 -- 3896. doi : 10.1021 / ja00193a021. Jump up ^ Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990. Jump up ^ Zug KA, Warshaw EM, Fowler JF Jr, Maibach HI, Belsito DL, Pratt MD, Sasseville D, Storrs FJ, Taylor JS, Mathias CG, Deleo VA, Rietschel RL, Marks J. Patch - test results of the North American Contact Dermatitis Group 2005 -- 2006. Dermatitis. 2009 May -- Jun ; 20 ( 3 ) : 149 - 60. Jump up ^ W. Jelkmann : The disparate roles of cobalt in erythropoiesis, and doping relevance. Open Journal of Hematology, 2012, 3 -- 6. http://rossscience.org/ojhmt/2075-907X-3-6.php Jump up ^ Lippi G, Franchini M, Guidi GC ( November 2005 ). `` Cobalt chloride administration in athletes : a new perspective in blood doping ? ''. Br J Sports Med. 39 ( 11 ) : 872 -- 3. doi : 10.1136 / bjsm. 2005.019232. PMC 1725077. PMID 16244201. External links Wikimedia Commons has media related to cobalt ( II ) chloride. International Chemical Safety Card 0783 National Pollutant Inventory -- Cobalt fact sheet IARC Monograph `` Cobalt and Cobalt Compounds '' Cobalt compounds CoBr Co ( CN ) CoCO CoC O CoCl CoCl Co ( ClO ) CoF CoF CoI Co ( NO ) Co ( NO ) CoO Co ( OH ) CoS CoSO CoSe Co O Co P Co O Co ( PO ) Retrieved from `` https://en.wikipedia.org/w/index.php?title=Cobalt(II)_chloride&oldid=816618968 '' Categories : Cobalt compounds Inorganic compounds Chlorides Metal halides IARC Group 2B carcinogens Deliquescent substances Hidden categories : CS1 maint : Uses authors parameter Chemical articles with multiple compound IDs Multiple chemicals in an infobox that need indexing Chemical articles with multiple CAS registry numbers Articles without KEGG source Articles with changed CASNo identifier ECHA InfoCard ID from Wikidata Chembox having DSD data Articles containing unverified chemical infoboxes All articles with unsourced statements Articles with unsourced statements from June 2010 Commons category with local link different than on Wikidata Talk Contents About Wikipedia تۆرکجه Català Čeština Deutsch Ελληνικά فارسی Français हिन्दी Italiano עברית Magyar Nederlands 日本 語 Polski Português Română Русский Simple English Slovenčina Српски / srpski Srpskohrvatski / српскохрватски Suomi தமிழ் తెలుగు Tiếng Việt 中文 Edit links This page was last edited on 22 December 2017, at 14 : 52. 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Question: what is the formula of cobalt(ii) chloride hexahydrate
Answer: CoCl2·6H2O