Import Question JSON

$\text{Step 1:}$ $\text{As the oxidation state of the central atom increases the acidity of the compound also increases.}$ $\text{Step 2:}$ $\text{The oxidation state of the central atoms in the given compounds is as follows:}$ $\text{HClO}_2 < \text{HClO}_3 < \text{HClO}_4$ $\text{+3} \quad \text{+5} \quad \text{+7}$ $\text{The electronegativity increases along the period. Acidity of hydrides of corresponding elements also increase with increase in electronegativity of these elements.}$ $\text{CH}_4 < \text{NH}_3 < \text{H}_2\text{O} < \text{HF}$ $\text{-4} \quad \text{-3} \quad \text{-2} \quad \text{-1}$ $\text{In the case of oxoacid of phosphorus, the above rule is not valid it is an exceptional case.}$ $\text{H}_3\text{PO}_4 < \text{H}_3\text{PO}_3 < \text{H}_3\text{PO}_2$ $\text{Phosphorous acid H}_3\text{PO}_3\text{: } 5.0 \times 10^{-2}$ $\text{Phosphoric acid H}_3\text{PO}_4\text{: } 6.9 \times 10^{-3}$ $\text{The double bonded oxygen has negative inductive effect (-I). And this electron withdrawing effect is experienced by one HH of the one -OH group in H}_3\text{PO}_2\text{. Hence it has the greatest acidic strength.}$ $\text{Similarly, the -I effect of OO is experienced by two HH of the two -OH groups in H}_3\text{PO}_3\text{, hence the electron-withdrawing effect is reduced because it is getting distributed between two groups. Hence, it has lesser acidic strength. Similarly, in H}_3\text{PO}_4\text{, it is distributed between 3 groups and so the acidic strength is the least.}$