Question
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-?
HClO_3^-?
H2SO4?
CO_3^2-?
Answers
GPT-4o mini
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
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