Which of the following is Bronsted Lowery acid base reaction?
Correct answer: C. HCl(g) + NH₃(g) → NH₄⁺ + Cl⁻
- A. NH₃ + BF₃ → NH₃BF₃
- B. HCl(aq) + NaOH(aq) → NaCl + H₂O
- C. HCl(g) + NH₃(g) → NH₄⁺ + Cl⁻
- D. All of the above
Explanation
The correct answer is Option C: HCl(g) + NH₃(g) → NH₄⁺ + Cl⁻. This reaction exemplifies a Bronsted-Lowry acid-base reaction because HCl donates a proton to NH₃, making HCl the acid (proton donor) and NH₃ the base (proton acceptor). Option A describes a Lewis acid-base reaction involving electron pair donation, not proton transfer. Option B, while an acid-base reaction, is more representative of an Arrhenius acid-base reaction due to the involvement of hydroxide ions. Option D is incorrect because not all the reactions listed are Bronsted-Lowry acid-base reactions.
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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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