All of the following can act as Brønsted-Lowry acids in aqueous solution except:

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Multiple Choice

All of the following can act as Brønsted-Lowry acids in aqueous solution except:

Brønsted-Lowry acids are substances that donate protons in solution. In water, you can test each species by whether it can give up an H+ to water (or another base). Hydroiodic acid readily donates its proton, producing hydronium and iodide, so it acts as an acid in aqueous solution. Bicarbonate is amphiprotic; it can lose a proton to become carbonate, so it can function as an acid as well. Hydrogen sulfide donates a proton to water to form bisulfide and hydronium, so it also behaves as an acid. Ammonia, however, behaves as a Brønsted-Lowry base in water. It accepts a proton from water to form ammonium and hydroxide: NH3 + H2O ⇌ NH4+ + OH−. Because it accepts, not donates, a proton in aqueous solution, it does not act as an acid here.

Brønsted-Lowry acids are substances that donate protons in solution. In water, you can test each species by whether it can give up an H+ to water (or another base).

Hydroiodic acid readily donates its proton, producing hydronium and iodide, so it acts as an acid in aqueous solution. Bicarbonate is amphiprotic; it can lose a proton to become carbonate, so it can function as an acid as well. Hydrogen sulfide donates a proton to water to form bisulfide and hydronium, so it also behaves as an acid.

Ammonia, however, behaves as a Brønsted-Lowry base in water. It accepts a proton from water to form ammonium and hydroxide: NH3 + H2O ⇌ NH4+ + OH−. Because it accepts, not donates, a proton in aqueous solution, it does not act as an acid here.

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