Q17 / 150 · MHT CET 2026 (15 April Shift 1) · Chemistry
Identify the strongest base according to Bronsted-Lowry theory from following.
- A$\text{Cl}^-$
- Correct answerB$\text{CH}_3\text{COO}^-$
- C$\text{NO}_3^-$
- D$\text{HSO}_4^-$
Solution
According to the Bronsted-Lowry theory, a stronger base has a weaker conjugate acid.
The conjugate acids of the given bases are:
$\text{Cl}^- \rightarrow \text{HCl}$ (strong acid)
$\text{CH}_3\text{COO}^- \rightarrow \text{CH}_3\text{COOH}$ (weak acid)
$\text{NO}_3^- \rightarrow \text{HNO}_3$ (strong acid)
$\text{HSO}_4^- \rightarrow \text{H}_2\text{SO}_4$ (strong acid)
Since $\text{CH}_3\text{COOH}$ is the weakest acid among the given conjugate acids, its conjugate base $\text{CH}_3\text{COO}^-$ is the strongest base.
Answer: $\text{CH}_3\text{COO}^-$
The conjugate acids of the given bases are:
$\text{Cl}^- \rightarrow \text{HCl}$ (strong acid)
$\text{CH}_3\text{COO}^- \rightarrow \text{CH}_3\text{COOH}$ (weak acid)
$\text{NO}_3^- \rightarrow \text{HNO}_3$ (strong acid)
$\text{HSO}_4^- \rightarrow \text{H}_2\text{SO}_4$ (strong acid)
Since $\text{CH}_3\text{COOH}$ is the weakest acid among the given conjugate acids, its conjugate base $\text{CH}_3\text{COO}^-$ is the strongest base.
Answer: $\text{CH}_3\text{COO}^-$
Hence, the correct answer is option: 'B'.