Question

Which net ionic equations demonstrate the Brønsted-Lowry acid character?

a) HCl + H₂O ⟶ Cl⁻ + H₃O⁺
b) NH₄⁺ + H₂O ⟶ NH₃ + H₃O⁺
c) HSO₄⁻ + OH⁻ ⟶ SO₄²⁻ + H₂O
d) H₂O + e⁻ ⟶ OH⁻ + H⁺

Answer 1

Brønsted-Lowry acids are characterized by their ability to donate protons. HNO3, PH2+, and H2S are examples of such acids, depicted through their respective reactions with water where they donate protons and form H3O+ ions.

Step-by-step explanation:

The Brønsted-Lowry acid concept defines an acid as a substance that can donate a proton (H+ ion), and a base as one that can accept a proton. To demonstrate how species can act as a Brønsted-Lowry acid, we look for reactions where the species donates a proton to another species.

• For HNO3: HNO3 (aq) + H2O(l) → NO3⁻ (aq) + H3O+ (aq)
• For PH2+: PH2+ (aq) + H2O(l) → PH3 (g) + H3O+ (aq)
• For H2S: H2S (aq) + H2O(l) → HS⁻ (aq) + H3O+ (aq)

Each reaction above involves a Brønsted-Lowry acid (HNO3, PH2+, or H2S) donating a proton to water, illustrating its acidic character.