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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. [22] 4 BF 3 + 3 H 2 O → 3 H[BF 4] + B(OH) 3. The heavier trihalides do not undergo analogous reactions, possibly due to the lower stability of the tetrahedral ions [BCl 4] − and [BBr 4] −.
Boron trifluoride etherate, strictly boron trifluoride diethyl etherate, or boron trifluoride–ether complex, is the chemical compound with the formula BF 3 O(C 2 H 5) 2, often abbreviated BF 3 OEt 2.
Pure H[BF 4] has not been described. The same holds true for the superacids that are known by the simplified formulas H[PF 6] and H[SbF 6]. [4] [5] However, a solution of BF 3 in HF is highly acidic, having an approximate speciation of [H 2 F] + [BF 4] − (fluoronium tetrafluoroborate) and a Hammett acidity function of −16.6 at 7 mol % BF 3, easily qualifying as a superacid. [6]
For liquid anydrous BF3, Carl Yaws' Chemical Properties Handbook liquid density curve ranges from 0.549 g/cm3 at critical temperature (-12.3 C) to 1.678 g/cm3 at -127 C, with 1.572 g/cm3 at atmospheric boiling point. Anhydrous BF3 can't be liquefied at 25 C, new density is ideal-gas density at 25 C and 100 kPa.
In chemistry, an acid–base reaction is a chemical reaction that occurs between an acid and a base.It can be used to determine pH via titration.Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.
A Lewis base is also a Brønsted–Lowry base, but a Lewis acid does not need to be a Brønsted–Lowry acid. The classification into hard and soft acids and bases ( HSAB theory ) followed in 1963. The strength of Lewis acid-base interactions, as measured by the standard enthalpy of formation of an adduct can be predicted by the Drago–Wayland ...
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The Hammett acidity function (H 0) is a measure of acidity that is used for very concentrated solutions of strong acids, including superacids.It was proposed by the physical organic chemist Louis Plack Hammett [1] [2] and is the best-known acidity function used to extend the measure of Brønsted–Lowry acidity beyond the dilute aqueous solutions for which the pH scale is useful.