A solution is created by mixing $250\,\mathrm{mL}$ of $1\,\mathrm{M}$ $\ce{HCl}$, $250\,\mathrm{mL}$ of $1\,\mathrm{M}$ $\ce{CH3COOH}$ and $500\,\mathrm{mL}$ of $1.5\,\mathrm{M}$ $\ce{CsOH}$.
The $K_\mathrm{a}(\ce{CH3COOH}) = 1.8 \times 10^{-5}$
What is the $\mathrm{pH}$ of this solution?
I am stuck between $\ce{HCl}$ and $\ce{CsOH}$ since they are both a strong acid and base (respectively) meaning that they should both have a substantial affect on the $\mathrm{pH}$.
Also when determining what the $\mathrm{pH}$ is, which species would we use in our ICE table?