Question
Question
For the reaction CH3COOH → CH3COO– + H+, which statement is true?
Responses
CH3COO– is a Lewis acid.
upeprcase C H subscript 3 end subscript uppercase C O O superscript minus end superscript is a Lewis acid.
CH3COOH is a Brønsted-Lowry acid.
uppercase C H subscript 3 end subscript uppercase C O O H is a Brønsted-Lowry acid.
CH3COO– is a conjugate acid.
uppercase C H subscript 3 end subscript uppercase C O O superscript minus end superscript is a conjugate acid.
CH3COO– is an Arrhenius base.
For the reaction CH3COOH → CH3COO– + H+, which statement is true?
Responses
CH3COO– is a Lewis acid.
upeprcase C H subscript 3 end subscript uppercase C O O superscript minus end superscript is a Lewis acid.
CH3COOH is a Brønsted-Lowry acid.
uppercase C H subscript 3 end subscript uppercase C O O H is a Brønsted-Lowry acid.
CH3COO– is a conjugate acid.
uppercase C H subscript 3 end subscript uppercase C O O superscript minus end superscript is a conjugate acid.
CH3COO– is an Arrhenius base.
Answers
GPT-4o mini
The correct statement regarding the reaction \( \text{CH}_3\text{COOH} \rightarrow \text{CH}_3\text{COO}^- + \text{H}^+ \) is:
**\( \text{CH}_3\text{COOH} \) is a Brønsted-Lowry acid.**
This is because in this reaction, acetic acid (\( \text{CH}_3\text{COOH} \)) donates a proton (\( \text{H}^+ \)) to form the acetate ion (\( \text{CH}_3\text{COO}^- \)). In Brønsted-Lowry theory, acids are defined as proton donors.
Other incorrect options include:
- \( \text{CH}_3\text{COO}^- \) is not a Lewis acid; it is a base since it accepts a proton.
- \( \text{CH}_3\text{COO}^- \) is not a conjugate acid; it is actually the conjugate base of acetic acid.
- \( \text{CH}_3\text{COO}^- \) is not an Arrhenius base, as it does not produce \( \text{OH}^- \) in water.
So the only true statement among the given options is that **\( \text{CH}_3\text{COOH} \) is a Brønsted-Lowry acid.**
**\( \text{CH}_3\text{COOH} \) is a Brønsted-Lowry acid.**
This is because in this reaction, acetic acid (\( \text{CH}_3\text{COOH} \)) donates a proton (\( \text{H}^+ \)) to form the acetate ion (\( \text{CH}_3\text{COO}^- \)). In Brønsted-Lowry theory, acids are defined as proton donors.
Other incorrect options include:
- \( \text{CH}_3\text{COO}^- \) is not a Lewis acid; it is a base since it accepts a proton.
- \( \text{CH}_3\text{COO}^- \) is not a conjugate acid; it is actually the conjugate base of acetic acid.
- \( \text{CH}_3\text{COO}^- \) is not an Arrhenius base, as it does not produce \( \text{OH}^- \) in water.
So the only true statement among the given options is that **\( \text{CH}_3\text{COOH} \) is a Brønsted-Lowry acid.**