Sodium tetrafluoroborate

Last updated
Sodium tetrafluoroborate
The sodium cation Sodium-3D.png
The sodium cation
The tetrafluoroborate anion (ball-and-stick model) Tetrafluoroborate-ion-3D-balls.png
The tetrafluoroborate anion (ball-and-stick model)
Names
Other names
sodium fluoroborate, NaBF4
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.931 OOjs UI icon edit-ltr-progressive.svg
PubChem CID
UNII
  • InChI=1S/BF4.Na/c2-1(3,4)5;/q-1;+1
  • [B-](F)(F)(F)F.[Na+]
Properties
NaBF4
Molar mass 109.794 g/mol
Density 2.47 g/cm3
Melting point 384 °C (723 °F; 657 K)
Related compounds
Other cations
Nitrosonium tetrafluoroborate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Sodium tetrafluoroborate is an inorganic compound with formula NaBF4. It is a salt that forms colorless or white rhombic crystals and is soluble in water (108 g/100 mL) but less soluble in organic solvents. [1]

Contents

Sodium tetrafluoroborate is used in some fluxes used for brazing and to produce boron trifluoride. [2]

Preparation

Sodium tetrafluoroborate can be prepared by neutralizing tetrafluoroboric acid with sodium carbonate or sodium hydroxide. [3]

NaOH + HBF4 → NaBF4 + H2O
Na2CO3 + 2 HBF4 → 2 NaBF4 + H2O + CO2

Alternatively the chemical can be synthesized from boric acid, hydrofluoric acid, and sodium carbonate: [2]

2H3BO3 + 8HF + Na2CO3 → 2NaBF4 + 7H2O + CO2

Reactions and uses

On heating to its melting point, sodium tetrafluoroborate decomposes to sodium fluoride and boron trifluoride: [4]

NaBF4 → NaF + BF3

It is a source of tetrafluoroborate anion, which is used in organic chemistry for the preparation of salts. Sodium tetrafluoroborate can be used for synthesis of ionic liquids, where tetrafluoroborate is the anion.

References

  1. ↑ Milne, G. W. A (2005-07-11). Gardner's Commercially Important Chemicals: Synonyms, Trade Names, and Properties. John Wiley & Sons. ISBN   9780471735182.
  2. 1 2 Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. New York: Academic Press. p. 220 & 222. ISBN   978-0121266011.{{cite book}}: ISBN / Date incompatibility (help)
  3. ↑ Eagleson, Mary (1994). Concise Encyclopedia Chemistry. Walter de Gruyter. ISBN   9783110114515.
  4. ↑ Richard J. Lewis, Sr (2008-07-14). Hazardous Chemicals Desk Reference. Wiley. ISBN   9780470334454.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.