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Chemical compound From Wikipedia, the free encyclopedia
Beryllium hydroxide, Be(OH)2, is an amphoteric hydroxide, dissolving in both acids and alkalis. Industrially, it is produced as a by-product in the extraction of beryllium metal from the ores beryl and bertrandite.[7] The natural pure beryllium hydroxide is rare (in form of the mineral behoite, orthorhombic) or very rare (clinobehoite, monoclinic).[8][9] When alkali is added to beryllium salt solutions the α-form (a gel) is formed. If this left to stand or boiled, the rhombic β-form precipitates.[10] This has the same structure as zinc hydroxide, Zn(OH)2, with tetrahedral beryllium centers.[11]
Names | |
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IUPAC name
Beryllium hydroxide | |
Other names
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Identifiers | |
3D model (JSmol) |
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ChEBI | |
ChemSpider | |
ECHA InfoCard | 100.033.048 |
EC Number |
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1024 | |
MeSH | Beryllium+hydroxide |
PubChem CID |
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RTECS number |
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UNII | |
CompTox Dashboard (EPA) |
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Properties | |
BeH2O2 | |
Molar mass | 43.026 g·mol−1 |
Appearance | Vivid white, opaque crystals |
Density | 1.92 g cm−3[1] |
Melting point | (decomposes) |
0.0000023965 g/L | |
Solubility product (Ksp) |
6.92×10−22[2] |
Acidity (pKa) | 3.7[3] |
Structure | |
Linear | |
Thermochemistry | |
Heat capacity (C) |
1.443 J K−1 |
Std molar entropy (S⦵298) |
47 J·mol−1·K−1[4] |
Std enthalpy of formation (ΔfH⦵298) |
-904 kJ mol−1[4] |
Gibbs free energy (ΔfG⦵) |
-818 kJ/mol |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards |
Carcinogenic |
GHS labelling: | |
[5] | |
Danger | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
4 mg kg−1 (intravenous, rat) |
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)[6] |
REL (Recommended) |
Ca C 0.0005 mg/m3 (as Be)[6] |
IDLH (Immediate danger) |
Ca [4 mg/m3 (as Be)][6] |
Related compounds | |
Related compounds |
Aluminium oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Beryllium hydroxide is difficult to dissolve in water. With alkalis it dissolves to form the tetrahydroxoberyllate (also known as tetrahydroxidoberyllate) anion, [Be(OH)4]2−.[12] With sodium hydroxide solution:
With acids, beryllium salts are formed.[12] For example, with sulfuric acid, H2SO4, beryllium sulfate is formed:
Beryllium hydroxide dehydrates at 400 °C to form the soluble white powder, beryllium oxide:[12]
Further heating at higher temperature produces acid insoluble BeO.[12]
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