Question

Use structure arguments to indentify the weakest acid in this group: HClO, HClO3, HBrO, HBrO3.

Answer 1

Discard 1: Among the halogens that make up the acid:

As the halogen atom is larger, the polarity of the acid increases, making it easier for the H + ion to detach from the molecule. Then, the acids with Cl- would be the weakest.

For oxacids, the oxygen atom creates a bridge between the halogen and the H + ion, for more electronegative halogens, then the strength of the acid increases.

In our case, HBrO and HBrO3 would be the weakest because they are oxacids.

Discard 2: Enter the quantity of oxygenates of the oxyacid:

The greater the amount of oxygen in the oxacid, the greater its strength.

In our case, leaving HBrO as the weakest acid in the group.