The proton acceptor is:
Correct answer: A. NH3
- A. NH3
- B. BF3
- C. HCl
- D. H+
Explanation
According to the Bronsted-Lowry theory, a base is a substance that accepts protons. NH3 is a classic example of a weak base that acts as a proton acceptor. In water, it reacts to form NH4+ and OH- ions, demonstrating its ability to accept a proton. In contrast, BF3 is a Lewis acid that accepts electron pairs, not protons. HCl is a proton donor, releasing H+ ions in water, and is therefore classified as an acid. Lastly, H+ is already a proton, so it cannot act as a proton acceptor.
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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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