Which of the following is not Bronsted-Lowery acid?
Correct answer: B. AlCl₃
- A. NH₄⁺
- B. AlCl₃
- C. H₂O
- D. H⁺
Explanation
The correct answer is AlCl₃. AlCl₃ functions as a Lewis acid by accepting electron pairs, but it does not donate protons, which is the defining characteristic of a Bronsted-Lowry acid. In contrast, NH₄⁺ can donate a proton to become NH₃, H₂O can donate a proton to become OH⁻, and H⁺ is itself a proton, making these substances Bronsted-Lowry acids.
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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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