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What is the formula for the conjugate acid of the Brønsted-Lowry base CH3NH2?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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In the Brønsted–Lowry model, what is the conjugate base of (ammonium)?
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Recall that in the Brønsted–Lowry acid-base theory, an acid is a proton (H⁺) donor and a base is a proton acceptor.
Identify the species given: ammonium ion, \(\mathrm{NH_4^+}\), which can act as an acid by donating a proton.
Determine the conjugate base by removing one proton (H⁺) from the acid \(\mathrm{NH_4^+}\).
Removing one proton from \(\mathrm{NH_4^+}\) results in \(\mathrm{NH_3}\), which is the conjugate base.
Therefore, the conjugate base of \(\mathrm{NH_4^+}\) is \(\mathrm{NH_3}\).
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