[dpm]

I see the general trend: the higher the oxidation state of the anion, the more acidic the molecule is (in general), but why? I imagine it has something to do with the net dipole and how tightly bound the H is to the Cl, but I just can't seem to wrap my head around it.

K(sub)a    for    HClO4 > HClO3 > HClO2 > HClO

Why?

[vhpk]

I see the general trend: the higher the oxidation state of the anion, the more acidic the molecule is (in general), but why? I imagine it has something to do with the net dipole and how tightly bound the H is to the Cl, but I just can't seem to wrap my head around it.

K(sub)a    for    HClO4 > HClO3 > HClO2 > HClO

Why?

HClO -> H⁺ + ClO^-
HClO₂ -> H⁺ + ClO₂^-
O is a more electronegative element than chlorine, it's an electron-withdrawing group too, when it's attached to Cl atom, it will disperse the negative chare on oxygen atom adjacent to Cl, hence stabilise the anion -> the more dissociations, the more acidic property