Beryllium sulfate

Beryllium sulfate

Identifiers
CAS Number	13510-49-1 N[???] 7787-56-6 (tetrahydrate) N
3D model (JSmol)	Interactive image
ChEBI	CHEBI:53473 Y
ChemSpider	24291 Y
ECHA InfoCard	100.033.478
EC Number	236-842-2
PubChem CID	26077
RTECS number	DS4800000
InChI InChI=1S/Be.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Y Key: KQHXBDOEECKORE-UHFFFAOYSA-L Y InChI=1/Be.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Key: KQHXBDOEECKORE-NUQVWONBAA
SMILES [Be+2].[O-]S([O-])(=O)=O
Properties[1]
Chemical 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 (230 °F; 383 K) (tetrahydrate, −2H2O) 400 °C (dihydrate, dehydr.) 550–600 decomposes
Boiling point	2,500 °C (4,530 °F; 2,770 K) (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 (ΔfG˚)	-1088 kJ/mol
Hazards
Safety data sheet	ICSC 1351
GHS pictograms
GHS signal word	DANGER
GHS hazard statements	H350, H330, H301, H372, H319, H335, H315, H317, H411
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	82 mg/kg (rat, oral) 80 mg/kg (mouse, oral)[2]
US health exposure limits (NIOSH):
PEL (Permissible)	TWA 0.002 mg/m3 C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[3]
REL (Recommended)	Ca C 0.0005 mg/m3 (as Be)[3]
IDLH (Immediate danger)	Ca [4 mg/m3 (as Be)][3]
Related compounds
Other cations	Magnesium sulfate Calcium sulfate Strontium sulfate Barium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Beryllium sulfate normally encountered as the tetrahydrate, [Be(H₂O)₄]SO₄ is a white crystalline solid. It was first isolated in 1815 by Jons Jakob Berzelius.^[4]

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.^[5] The tetrahydrate contains a tetrahedral Be(OH₂)₄²⁺ unit and sulfate anions. The small size of the Be²⁺ cation determines the number of water molecules that can be coordinated. This contrasts with the analogous magnesium salt, MgSO₄·6H₂O which contains an octahedral Mg(OH₂)₆²⁺ unit.^[6]

The anhydrous compound has a structure similar to that of berlinite. The structure contains alternating tetrahedrally coordinated Be and S and each oxygen is 2 coordinate (Be-O-S). The Be-O distance is 156 pm and the S-O distance is 150 pm.^[7]

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

References

External links

• International Chemical Safety Card 1351
• IARC Monograph "Beryllium and Beryllium Compounds"
• IPCS Health & Safety Guide 44
• IPCS Environmental Health Criteria 106: Beryllium
• IPCS CICAD 32