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assify each species as either a Bronsted-Lowry acid, Bronsted-Lowry base, or as amphiprotic. Select the single best answer for each part.

HClO_3^-?
H2SO4?
CO_3^2-?

1 answer

To classify each of the given species according to the Bronsted-Lowry definitions:

  1. HClO₃⁻ (Chlorate ion): This species can accept a proton (H⁺) to form HClO₃ (chloric acid), but it doesn't easily donate a proton as it doesn't possess acidic protons. Therefore, it is best classified as a Bronsted-Lowry base.

  2. H₂SO₄ (Sulfuric acid): This species can donate a proton (H⁺) to form HSO₄⁻ (hydrogen sulfate ion). Thus, it is classified as a Bronsted-Lowry acid.

  3. CO₃²⁻ (Carbonate ion): This species can both accept a proton to form HCO₃⁻ (bicarbonate ion) and donate a proton to form CO₃²⁻ (since HCO₃⁻ can further donate a proton). As it can act as both an acid and a base, it is classified as amphiprotic.

To summarize:

  • HClO₃⁻: Bronsted-Lowry base
  • H₂SO₄: Bronsted-Lowry acid
  • CO₃²⁻: Amphiprotic