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23 lip 1999 · Hydrogen bonds from the solvating HF molecules help increase the Lewis acidity of BF 3 by utilizing the lone-pair electrons of its fluorine atoms. The crucial effect of the additional hydrogen-bonded HF molecules is reflected on the decrease in d BF .
In the case of BF3 and CaO you might predict you'd get a product like Ca[BF3O] -- the more canonical example is a borane like BH3 (a Lewis acid) reacting with an amine like ammonia (a Lewis base) to form the Lewis acid-base adduct amine-borane, H3N-BH3.
29 lis 2015 · Yes, the reason it is a Lewis acid is because BF3 must accept one more pair of electrons to have a full octet. This means that it will gain an H atom, so the pH will be lower because there is more hydrogen present.
12 paź 2016 · Two ionic equilibrium models were proposed to simulate the hydrolysis equilibrium of BF3 and tested by special acid-base titration technique. The most accurate ion equilibrium constants were determined.
The thermodynamics solvolysis constant of the BF 4 − ion in liquid anhydrous hydrogen fluoride was determined to be 7·7 × 10 −3 by a method of solubility measurements. From the extensive solvolysis of its salt, it was concluded, therefore, the BF 3 was not a strong acid in liquid HF.
The results essentially showed that the enthalpy of BF 3 adduct formation in DCM solution was clearly influenced by specific interactions, with DCM acting as hydrogen-bonding donor (HBD) molecule in two ways: base/DCM and adduct/DCM, confirming that specific solvation is an important contribution to experimentally determined Lewis basicity ...
Boron trifluoride reacts with water to give boric acid and fluoroboric acid. The reaction commences with the formation of the aquo adduct, H 2 O−BF 3 , which then loses HF that gives fluoroboric acid with boron trifluoride.
