Which of the following is not Bronsted-Lowery base?
Correct answer: C. BF₃
- A. H₂O
- B. HCO₃⁻
- C. BF₃
- D. ROH
Explanation
The correct answer is BF₃ because a Bronsted-Lowry base is defined as a substance that can accept a proton (H⁺). BF₃ does not accept protons; instead, it acts as a Lewis acid by accepting electron pairs. Conversely, H₂O, HCO₃⁻, and ROH can all accept a proton, fitting the definition of Bronsted-Lowry bases.
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About Acids, Bases and Salts
Acid and base behaviour is explained through the Bronsted-Lowry transfer of protons and the Lewis donation or acceptance of electron pairs. The topic includes pH, pOH, ionisation and water equilibrium, plus salt formation and hydrolysis, where a salt solution may become acidic, basic or neutral.
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