Multiple Choice
The following equation shows the equilibrium in an aqueous solution of ethylamine:C2H5NH2(aq) + H2O(l) ⇌ C2H5NH3+(aq) + OH−(aq)Which of the following represents a conjugate acid-base pair?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
Multiple Choice
In the Brønsted–Lowry acid–base model, what is the conjugate acid of (ammonia)?
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Verified step by step guidance1
Recall that in the Brønsted–Lowry acid–base model, a base is a species that accepts a proton (H⁺), and its conjugate acid is the species formed after it gains that proton.
Identify the given base: ammonia, which has the chemical formula \(\mathrm{NH_3}\).
To find the conjugate acid of ammonia, add one proton (H⁺) to the ammonia molecule, increasing the number of hydrogen atoms by one.
Write the formula of the conjugate acid by adding the proton to ammonia: \(\mathrm{NH_3} + \mathrm{H^+} \rightarrow \mathrm{NH_4^+}\).
Note that the conjugate acid has one more hydrogen and carries a positive charge due to the added proton, so the conjugate acid of ammonia is \(\mathrm{NH_4^+}\).
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