What's the order of oxidising strength of the oxyacids of Chlorine?
For many acids, the proton $\ce{H+}$ is the oxidizing agent. For example, in the oxidation of zinc with $\ce{HCl}$, the oxidizing agent is $\ce{H+}$.

$$\ce{Zn + 2H+ -&gt; Zn^{2+} + H2}$$

However, for some acids, the conjugate base (anion) is also an oxidant (and usually a more powerful oxidant than $\ce{H+}$. The oxyacids of chlorine are all oxidizing agents through their anions, as is nitric acid and some others:

$$\ce{Zn + 2H+ + 2OCl- -&gt; Zn^{2+} + H2O + 2Cl-}$$

In the above example, hypochlorite is the oxidizing agent. For the oxyacids of chlorine and others, the strength of the oxidizing agent is independent of the strength of the acid.