Which of the following is not a Bronsted acid

Options

A. `NH_(4)^(+)`
B. `HCO_(3)^(-)`
C. `HCO_(3)^(-)`
D. `CH_(3)COO^(-)`

Explanation

To determine which of the following options is not a Bronsted acid, we will analyze each option based on the Bronsted-Lowry theory, which defines an acid as a species that donates a proton (H⁺) and a base as a species that accepts a proton.

### Step-by-Step Solution:

1. **Understanding Bronsted Acids**:
- According to the Bronsted-Lowry theory, an acid is any substance that can donate a proton (H⁺). Therefore, to identify which option is not a Bronsted acid, we need to check if each option can donate a proton.

2. **Analyzing Each Option**:
- **Option 1: NH₄⁺ (Ammonium Ion)**:
- When NH₄⁺ reacts with water, it donates a proton to water, forming NH₃ (ammonia) and H₃O⁺ (hydronium ion):
\[ NH₄^+ + H₂O \rightarrow NH₃ + H₃O^+ \]
- Since NH₄⁺ donates a proton, it is a Bronsted acid.

- **Option 2: HCO₃⁻ (Bicarbonate Ion)**:
- When HCO₃⁻ reacts with water, it can also donate a proton, forming CO₃²⁻ (carbonate ion) and H₃O⁺:
\[ HCO₃^- + H₂O \rightarrow CO₃^{2-} + H₃O^+ \]
- Therefore, HCO₃⁻ is also a Bronsted acid.

- **Option 3: CH₃COO⁻ (Acetate Ion)**:
- The acetate ion (CH₃COO⁻) does not have a proton to donate. It is the conjugate base of acetic acid (CH₃COOH) and cannot donate a proton:
\[ CH₃COO^- \text{ has no H⁺ to donate.} \]
- Thus, CH₃COO⁻ is not a Bronsted acid.

- **Option 4: CH₃CO⁻ (Hypothetical Ion)**:
- The notation CH₃CO⁻ is not standard; however, if we assume it refers to a similar structure without a proton to donate, it would also not be a Bronsted acid. But since we have already identified CH₃COO⁻ as not being a Bronsted acid, we can conclude that this option is also not a Bronsted acid.

3. **Conclusion**:
- The only species among the options that does not donate a proton is CH₃COO⁻. Therefore, the answer to the question "Which of the following is not a Bronsted acid?" is **CH₃COO⁻**.

### Final Answer:
**CH₃COO⁻ (Acetate Ion) is not a Bronsted acid.**