Q130 / 200 · MHT CET - Medical 2026 (21 April Shift 1) · Chemistry
Identify the correct order of acidity of the following compounds.
- A$\text{HClO}_2 < \text{HClO} < \text{HClO}_3 < \text{HClO}_4$
- B$\text{HClO}_4 < \text{HClO}_2 < \text{HClO} < \text{HClO}_3$
- C$\text{HClO}_3 < \text{HClO}_4 < \text{HClO}_2 < \text{HClO}$
- Correct answerD$\text{HClO} < \text{HClO}_2 < \text{HClO}_3 < \text{HClO}_4$
Solution
The acidic strength of oxoacids of the same halogen increases with an increase in the oxidation state of the halogen atom.
The oxidation states of chlorine in the given oxoacids are:
$\text{HClO}$: $+1$
$\text{HClO}_2$: $+3$
$\text{HClO}_3$: $+5$
$\text{HClO}_4$: $+7$
As the oxidation state of the central chlorine atom increases, its electronegativity increases. This increases the polarization of the $\text{O-H}$ bond, facilitating the release of an $\text{H}^+$ ion.
Additionally, the stability of the conjugate base increases with the number of oxygen atoms due to greater resonance stabilization ($\text{ClO}^- < \text{ClO}_2^- < \text{ClO}_3^- < \text{ClO}_4^-$).
Thus, the correct order of acidic strength is $\text{HClO} < \text{HClO}_2 < \text{HClO}_3 < \text{HClO}_4$.
Answer: $\text{HClO} < \text{HClO}_2 < \text{HClO}_3 < \text{HClO}_4$
The oxidation states of chlorine in the given oxoacids are:
$\text{HClO}$: $+1$
$\text{HClO}_2$: $+3$
$\text{HClO}_3$: $+5$
$\text{HClO}_4$: $+7$
As the oxidation state of the central chlorine atom increases, its electronegativity increases. This increases the polarization of the $\text{O-H}$ bond, facilitating the release of an $\text{H}^+$ ion.
Additionally, the stability of the conjugate base increases with the number of oxygen atoms due to greater resonance stabilization ($\text{ClO}^- < \text{ClO}_2^- < \text{ClO}_3^- < \text{ClO}_4^-$).
Thus, the correct order of acidic strength is $\text{HClO} < \text{HClO}_2 < \text{HClO}_3 < \text{HClO}_4$.
Answer: $\text{HClO} < \text{HClO}_2 < \text{HClO}_3 < \text{HClO}_4$
Hence, the correct answer is option: 'D'.