객관식
In the Brønsted–Lowry model, what is the conjugate base of after it donates a proton?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
객관식
In the Brønsted–Lowry definition, what is the conjugate base of the ammonium ion (often written as )?
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검증된 단계별 안내1
Recall the Brønsted–Lowry definition of acids and bases: an acid is a proton (H⁺) donor, and a base is a proton acceptor.
Identify the ammonium ion, \( \mathrm{NH_4^+} \), as the species that can donate a proton (H⁺) because it carries a positive charge and has an extra hydrogen compared to ammonia.
Determine the conjugate base by removing one proton (H⁺) from the ammonium ion. This means subtracting one hydrogen ion from \( \mathrm{NH_4^+} \).
Write the formula of the species left after the proton is removed. Removing one H⁺ from \( \mathrm{NH_4^+} \) results in \( \mathrm{NH_3} \), which is ammonia.
Conclude that the conjugate base of the ammonium ion \( \mathrm{NH_4^+} \) is ammonia, \( \mathrm{NH_3} \).
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