Answer
$$0.10 \space M \space HCl \gt 0.10 \space M \space HF \gt 0.10 \space M \space HClO \gt 0.10 \space M \space HC_6H_5O$$
Work Step by Step
Considering equal concentrations (0.10 M):
Since $HCl$ is the only strong acid in the list, it will be the one with greater $[H_3O^+]$, which is equal to 0.10 M. The other acids are weak, thus, they will not completely dissociate, and the $[H_3O^+]$ will be less than 0.10 M
$HC_6H_5O$, $HClO$ and $HF$, in order of decreasing $K_a$:
$$HF \gt HClO \gt HC_6H_5O$$
The greater the $K_a$, more dissociation, and more $[H_3O^+]$. Thus, these are the solutions in order of decreasing $[H_3O^+]$
$$0.10 \space M \space HCl \gt 0.10 \space M \space HF \gt 0.10 \space M \space HClO \gt 0.10 \space M \space HC_6H_5O$$
