Difference between revisions of "Beryllium sulfate"
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| Section2 = {{Chembox Properties | | Section2 = {{Chembox Properties | ||
| − | | Reference = <ref>{{RubberBible62nd|page=B-82}}.</ref> | + | | Reference = <ref name="RubberBible">{{RubberBible62nd|page=B-82}}.</ref> |
| Formula = BeSO<sub>4</sub> | | Formula = BeSO<sub>4</sub> | ||
| MolarMass = 105.075 g/mol (anhydrous)<br/> 177.136 g/mol (tetrahydrate) | | MolarMass = 105.075 g/mol (anhydrous)<br/> 177.136 g/mol (tetrahydrate) | ||
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| Section7 = {{Chembox Hazards | | Section7 = {{Chembox Hazards | ||
| − | | ExternalMSDS = | + | | Reference = <ref name="CLP">{{CLP Regulation|page=341}}</ref> |
| + | | ExternalMSDS = {{ICSC-small|1351}} | ||
| EUIndex = 004-002-00-2 | | EUIndex = 004-002-00-2 | ||
| − | + | | GHSPictograms = {{GHS06|Acute Tox. 2}}{{GHS08|Carc. 1B}}{{GHS09|Aquatic Chronic 2}} | |
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| − | | GHSPictograms = {{GHS06|Acute Tox. 2}} {{GHS08|Carc. 1B}} {{GHS09|Aquatic Chronic 2}} | ||
| GHSSignalWord = DANGER | | GHSSignalWord = DANGER | ||
| HPhrases = {{H-phrases|350|330|301|372|319|335|315|317|411}} | | HPhrases = {{H-phrases|350|330|301|372|319|335|315|317|411}} | ||
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| − | '''Beryllium sulfate''' (BeSO<sub>4</sub>) is a white crystalline solid. It was first isolated in 1815 by [[ | + | '''Beryllium sulfate''' (BeSO<sub>4</sub>) is a white crystalline solid. It was first isolated in 1815 by [[Jöns Jakob Berzelius]].<ref>{{citation | first = Charles | last = Lathrop Parsons | year = 1909 | title = The Chemistry and Literature of Beryllium | url = http://books.google.es/books?id=iI8vpmK7jgoC | location = London | pages = 29–33}}.</ref> |
Beryllium sulfate may be prepared by treating an aqueous solution of any beryllium salt with sulfuric acid, followed by evaporation of the solution and crystallization. The hydrated product may be converted to anhydrous salt by heating at 400 °C.<ref>{{citation | first = Pradyot | last = Patnaik | title = Handbook of Inorganic Chemicals | publisher = McGraw-Hill | year = 2002 | isbn = 0070494398}}.</ref> | Beryllium sulfate may be prepared by treating an aqueous solution of any beryllium salt with sulfuric acid, followed by evaporation of the solution and crystallization. The hydrated product may be converted to anhydrous salt by heating at 400 °C.<ref>{{citation | first = Pradyot | last = Patnaik | title = Handbook of Inorganic Chemicals | publisher = McGraw-Hill | year = 2002 | isbn = 0070494398}}.</ref> | ||
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==External links== | ==External links== | ||
*{{ICSC|1351}} | *{{ICSC|1351}} | ||
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| − | |||
*{{EHC|106|name=Beryllium}} | *{{EHC|106|name=Beryllium}} | ||
| − | * | + | *{{CICAD|32|name=Beryllium and Beryllium Compounds}} |
| + | *{{HSG|044|name=Beryllium}} | ||
| + | *{{IARC beryllium}} | ||
[[Category:Beryllium compounds]] | [[Category:Beryllium compounds]] | ||
Revision as of 04:53, 4 December 2009
| Beryllium sulfate | |
|---|---|
| Identifiers | |
| CAS number | [] |
| EC number | |
| RTECS | DS4800000 |
| PubChem | |
| Properties[1] | |
| Chemical formula | BeSO4 |
| Molar mass | 105.075 g/mol (anhydrous) 177.136 g/mol (tetrahydrate) |
| Appearance | white solid |
| Density | 2.50 g/cm3 (anhydrous) 1.71 g/cm3 (tetrahydrate) |
| Melting point |
110 °C (tetrahydrate, −2H2O) |
| Solubility in water | 30.5 g/100 mL (30 °C) |
| Solubility | insoluble in alcohol |
| Refractive index (nD) | 1.4374 (tetrahydrate) |
| Hazards[2] | |
| Material safety data sheet (MSDS) | ICSC |
| EU index number | 004-002-00-2 |
| GHS pictograms |   
|
| GHS signal word | DANGER |
| GHS hazard statements | H350, H330, H301, H372, H319, H335, H315, H317, H411 |
| Flash point | non-flammable |
| LD50 | 82 mg/kg |
| Related compounds | |
| Other cations | Magnesium sulfate Calcium sulfate Strontium sulfate Barium sulfate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Beryllium sulfate (BeSO4) is a white crystalline solid. It was first isolated in 1815 by Jöns Jakob Berzelius.[3]
Beryllium sulfate may be prepared by treating an aqueous solution of any beryllium salt with sulfuric acid, followed by evaporation of the solution and crystallization. The hydrated product may be converted to anhydrous salt by heating at 400 °C.[4]
A mixture of beryllium and radium sulfate was used as the neutron source in the discovery of nuclear fission.
References
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-82. ISBN 0-8493-0462-8.
- ↑ Regulation (EC) No 1272/2008 of the European Parliament and of the Council of 16 December 2008 on classification, labelling and packaging of substances and mixtures, amending and repealing Directives 67/548/EEC and 1999/45/EC, and amending Regulation (EC) No 1907/2006. OJEU L353, 31.12.2008, pp 1–1355 at p 341.
- ↑ Lathrop Parsons, Charles The Chemistry and Literature of Beryllium; London, 1909; pp 29–33, <http://books.google.es/books?id=iI8vpmK7jgoC>.
- ↑ Patnaik, Pradyot Handbook of Inorganic Chemicals; McGraw-Hill, 2002. ISBN 0070494398.
External links
- International Chemical Safety Card 1351
- IPCS Environmental Health Criteria 106: Beryllium
- IPCS Concise International Chemical Assessment Document 32: Beryllium and Beryllium Compounds
- IPCS Health and Safety Guide 044: Beryllium
- Beryllium and Beryllium Compounds. In Beryllium, Cadmium, Mercury, and Exposures in the Glass Manufacturing Industry; IARC Monographs on the Evaluation of Carcinogenic Risks to Humans 58; International Agency for Research on Cancer: Lyon, France, 1993; pp 41–117. ISBN 92-832-1258-4, <http://monographs.iarc.fr/ENG/Monographs/vol58/mono58-6.pdf>
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