Beryllium sulfate

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Beryllium sulfate
Beryllium sulfate.svg
Beryllium sulfate 4 hydrate.jpg
Identifiers
CAS number 13510-49-1 N[???], 7787-56-6 (tetrahydrate)
PubChem 26077
ChemSpider 24291 YesY
EC number 236-842-2
ChEBI CHEBI:53473 YesY
RTECS number DS4800000
Jmol-3D images Image 1
Properties[1]
Molecular formula BeSO4
Molar mass 105.075 g/mol (anhydrous)
177.136 g/mol (tetrahydrate)
Appearance white solid
Odor odorless
Density 2.44 g/cm3 (anhydrous)
1.71 g/cm3 (tetrahydrate)
Melting point 110 °C (tetrahydrate, −2H2O)
400 °C (dihydrate, dehydr.)
550–600 decomp.
Boiling point 2500 °C (anhydrate)
580 °C (tetrahydrate)
Solubility in water 36.2 g/100 mL (0 °C)
40.0 g/100 mL (20 °C)
54.3 g/100 mL (60 °C)
Solubility insoluble in alcohol
Refractive index (nD) 1.4374 (tetrahydrate)
Thermochemistry
Std molar
entropy
So298
90 J/mol K
Std enthalpy of
formation
ΔfHo298
-1197 kJ/mol
Gibbs free energy ΔG -1088 kJ/mol
Hazards
MSDS ICSC 1351
GHS pictograms Acute Tox. 2 Carc. 1B Aquatic Chronic 2
GHS signal word DANGER
GHS hazard statements H350, H330, H301, H372, H319, H335, H315, H317, H411
EU Index 004-002-00-2
EU classification Carc. Cat. 2
Very toxic (T+)
Dangerous for the environment (N)
R-phrases R49, R25, R26, R36/37/38, R43, R48/23, R51/53
S-phrases S53, S45
Flash point Non-flammable
LD50 82 mg/kg (rat, oral)
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 (77 °F), 100 kPa)
 N (verify) (what is: YesY/N?)
Infobox references

Beryllium sulfate (BeSO4) is a white crystalline solid. It was first isolated in 1815 by Jons Jakob Berzelius.[2]

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.[3]

A mixture of beryllium and radium sulfate was used as the neutron source in the discovery of nuclear fission.

References[edit]

  1. ^ Weast, Robert C., ed. (1981). CRC Handbook of Chemistry and Physics (62nd ed.). Boca Raton, FL: CRC Press. p. B-82. ISBN 0-8493-0462-8. .
  2. ^ Lathrop Parsons, Charles (1909), The Chemistry and Literature of Beryllium, London, pp. 29–33 .
  3. ^ Patnaik, Pradyot (2002), Handbook of Inorganic Chemicals, McGraw-Hill, ISBN 0-07-049439-8 .

External links[edit]