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Classify each species as either a Bronsted-Lowry acid, Bronsted-Lowry base, or as amphiprotic. Select the single best answer fo...Question
Classify each species as either a Bransted-Lowry acid, Brensted-Lowry base, or as amphiprotic. Select the single best answer for each part.
H2CO3?
H2PO^-_4?
PO^3-_4?
H2CO3?
H2PO^-_4?
PO^3-_4?
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Answered by
GPT-4o mini
Let's classify each species based on the Brønsted-Lowry acid-base theory.
1. **H2CO3 (Carbonic acid)**: This compound can donate a proton (H⁺) and acts as an acid. Therefore, it is classified as a **Brønsted-Lowry acid**.
2. **H2PO4⁻ (Dihydrogen phosphate ion)**: This species can both donate a proton (acting as an acid) and accept a proton (acting as a base). Therefore, it is classified as **amphiprotic**.
3. **PO4^3- (Phosphate ion)**: This species can accept a proton to form HPO4^2-, but does not donate a proton. Therefore, it acts only as a base in this context and is classified as a **Brønsted-Lowry base**.
To summarize:
- **H2CO3**: Brønsted-Lowry acid
- **H2PO4⁻**: Amphiprotic
- **PO4^3-**: Brønsted-Lowry base
1. **H2CO3 (Carbonic acid)**: This compound can donate a proton (H⁺) and acts as an acid. Therefore, it is classified as a **Brønsted-Lowry acid**.
2. **H2PO4⁻ (Dihydrogen phosphate ion)**: This species can both donate a proton (acting as an acid) and accept a proton (acting as a base). Therefore, it is classified as **amphiprotic**.
3. **PO4^3- (Phosphate ion)**: This species can accept a proton to form HPO4^2-, but does not donate a proton. Therefore, it acts only as a base in this context and is classified as a **Brønsted-Lowry base**.
To summarize:
- **H2CO3**: Brønsted-Lowry acid
- **H2PO4⁻**: Amphiprotic
- **PO4^3-**: Brønsted-Lowry base