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3D model (JSmol) |
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| ECHA InfoCard | 100.033.478 |
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| Properties[1] | |
| 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.) 550–600decomposes |
| Boiling point | 2,500 °C (4,530 °F; 2,770 K) (anhydrate) 580 °C (tetrahydrate) |
| 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(S⦵298) | 90 J/mol K |
Std enthalpy of formation(ΔfH⦵298) | −1197 kJ/mol |
Gibbs free energy(ΔfG⦵) | −1088 kJ/mol |
| Hazards | |
| GHS labelling: | |
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| Danger | |
| H301,H315,H317,H319,H330,H335,H350,H372,H411 | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 82 mg/kg (rat, oral) 80 mg/kg (mouse, oral)[3] |
| NIOSH (US health exposure limits): | |
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)[2] |
REL (Recommended) | Ca C 0.0005 mg/m3 (as Be)[2] |
IDLH (Immediate danger) | Ca [4 mg/m3 (as Be)][2] |
| Safety data sheet (SDS) | ICSC 1351 |
| Related compounds | |
Othercations | Magnesium sulfate Calcium sulfate Strontium sulfate Barium sulfate |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Beryllium sulfate normally encountered as the tetrahydrate, [Be(H2O)4]SO4 is a white crystalline solid. It was first isolated in 1815 byJons Jakob Berzelius.[4]Beryllium sulfate may be prepared by treating an aqueous solution of many beryllium salts withsulfuric acid, followed by evaporation of the solution and crystallization. The hydrated product may be converted toanhydrous salt by heating at 400 °C.[5]
According toX-ray crystallography 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.[6] In contrast, the analogous magnesium salt, MgSO4·6H2O contains an octahedral Mg(OH2)62+ unit.[7] The existence of the tetrahedral [Be(OH2)4]2+ ion in aqueous solutions ofberyllium nitrate andberyllium chloride has been confirmed byvibrational spectroscopy, as indicated by the totally symmetric BeO4 mode at 531 cm−1. This band is absent in beryllium sulfate, and the sulfate modes are perturbed. The data support the existence of Be(OH2)3OSO3.[8]
The anhydrous compound has a structure similar to that ofboron phosphate. 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.[9]
A mixture of beryllium andradium sulfate was used as theneutron source in the discovery ofnuclear fission.
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