Registration Dossier
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EC number: 220-543-9 | CAS number: 2802-68-8
Endpoint summary
Administrative data
Description of key information
Similar to all coordination complexes of boron trifluoride with organic and inorganic species (like alcohols, ethers, amines, sulfuric acid, sulfuric dioxide, etc) the complex of boron trifluoride and methanol is extremely water sensitive and reacts even with moist air.
In the instantaneous reaction with water as a first step methano land boron trifluoride dihydrateare formed.
BF3·CH3OH + 2 H2O -> BF3· 2 H2O + CH3OH
The hydrolysis of borontrifluoride dihydrate was investigated at pH-values of 1.2; 4.0; 7.0 and 9.0 (BASF SE, Study No. 09S01179, 26.19.2009)
The hydrolysis of the test item is a very fast process (half-life < 30 minutes). Already at room temperature about 30 to 60% of the test item was hydrolyzed within minutes in all tested buffer solutions in the pH range 1.2 to 9.0.
The main reactions of the hydrolysis process are the following:
BF3.2H2O + H2O → B(OH)3+ 3HF
HF + BF3.2H2O → HBF4+ 2H2O
B(OH)3+ 4HF → HBF4+ 3 H2O
HBF4+ H2O ↔ HBF3(OH) + HF
Total hydrolysis of HBF4:
HBF4↔ HBF3(OH) ↔ HBF2(OH)2↔ HBF(OH)3↔ HB(OH)4= B(OH)3+ H2O
Boric acid and tetrafluoroboratesare expected to be the main species in the dilute hydrolysis solution (Zhang Weijiang et al.).
In conclusion, given the very rapid hydrolysis reaction, it is considered justified to base the assessment of the toxicity of hydrogen trifluoromethoxyborate (1-), compound with methanol (1.1) to aquatic organisms on the properties of the breakdown products.
References:
BASF SE, Boron trifluoride dihydrate: hydrolysis as a function of pH, Study No. 09S01179, 26.10.2009
Wamser C. A. Equilibria in the system boron trifluoride-water at 25 °C, Journal of the American Chemical Society, 1951, 73: 409-416
Zhang Weijiang et al., Equilibrium on the hydrolysis of Boron trifluoride in large amount of water, Transactions of Tianjin University, 2016, 22: 486-491
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