Boron phosphate
Names
IUPAC name
Boron phosphate
Systematic IUPAC name
2,4,5-trioxa-1λ5-phospha-3-borabicyclo[1.1.1]pentane 1-oxide[1]
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.020 Edit this at Wikidata
  • InChI=1S/B.H3O4P/c;1-5(2,3)4/h;(H3,1,2,3,4)/q+3;/p-3
    Key: YZYDPPZYDIRSJT-UHFFFAOYSA-K
  • InChI=1/B.H3O4P/c;1-5(2,3)4/h;(H3,1,2,3,4)/q+3;/p-3
    Key: YZYDPPZYDIRSJT-DFZHHIFOAS
  • B12OP(=O)(O1)O2
Properties
BPO4
Molar mass 105.78 g/mol
Density 2.52 g/cm3
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H302
P264, P270, P301+P312, P330, P501
NFPA 704 (fire diamond)
[2]
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Safety data sheet (SDS) External SDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Boron phosphate is an inorganic compound with the chemical formula BPO4. The simplest way of producing it is the reaction of phosphoric acid and boric acid. It is a white infusible solid that evaporates above 1450 °C.[3]

Synthesis

Boron phosphate is synthesized from phosphoric acid and boric acid at a temperature range from 80 °C to 1200 °C. The relatively cold treatment produces a white amorphous powder, which is converted to a microcrystalline product when heated at about 1000 °C for 2 hours.[4]

The main reaction of the process is:

H3BO3 + H3PO4 → BPO4 + 3 H2O

New ways of synthesizing the compound have also been reported, such as hydrothermal and microwave synthesis.[5]

Due to the particular industrial interest of boron phosphate, other methods are used as well:[5]

Structure

If obtained at pressure, the ordinary structure is isomorphous with the β-cristobalite, while subjecting it to high pressure is obtained a compound isomorphic with α-quartz.[6] The structure of AlPO4, berlinite, is isomorphous with α-quartz.[3]

Applications

It is used as a catalyst for dehydration and other reactions in organic synthesis. Also, it serves as a source of phosphates for exchange reactions in the solid state to obtain metal phosphates.[7]

References

  1. ^ pubchem.ncbi.nlm.nih.gov/compound/83329#section=IUPAC-Name&fullscreen=true
  2. ^ Boron phosphate datasheets.scbt.com
  3. ^ a b Corbridge DEC 2013, Phosphorus: Chemistry, Biochemistry and Technology, 6th ed., CRC Press, Boca Raton, Florida, ISBN 978-1-4398-4088-7
  4. ^ Mylius, F.; Meusser, A. (1904). "Ueber die Bestimmung der Borsäure als Phosphat". Berichte der Deutschen Chemischen Gesellschaft. 37: 397–401. doi:10.1002/cber.19040370171.
  5. ^ a b Baykal, A; Kizilyalli, M; Toprak, Muhammet S. & Kniep, R (2001). "Hydrothermal and microwave synthesis of boron phosphate, BPO4". Turkish Journal of Chemistry. 25 (4): 425–432.
  6. ^ MacKenzie, J. D.; Roth, W. L.; Wentorf, R. H. (1959). "New high pressure modifications of BPO4 and BAsO4". Acta Crystallographica. 12 (1): 79. Bibcode:1959AcCry..12...79M. doi:10.1107/S0365110X5900024X.
  7. ^ Moffat, J. B.; Goltz, H. L. (1965). "Surface Chemistry and Catalytic Properties of Boron Phosphate: 1. Surface Area and Acidity". Canadian Journal of Chemistry. 43 (6): 1680. doi:10.1139/v65-222.
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