[page3333]

reactions for two cases
HX+H2O -> H3O+   + X-
HX+CH3COOH -> CH3COOH2+   + X-

I know that acidity(in water) of HI, HBr and HCl are almost indistinguishable(but actually dissociation rate is relatively HI>HBr>HCl) because of the leveling effect of water.
But in acetic acid we can rank acidities of these acids apparently, HI>HBr>HCl

I think this is because acetic acid has smaller dipole moment than that of water, so ability to dissociate two atoms in acid molecules of it is weaker.
Thus differences between dissociation rate of acids in acetic acid get bigger.

is this appropriate explanation?
 

[Babcock_Hall]

Which is easier to protonate, water or acetic acid?