Help with a difficult chemistry problem

If you have 500 mL of a 0.001 M HCl solution and you react it with 0.5 grams of Sr(OH)2, what is the pH of the resulting solution?

I set up the balanced equation:
Sr(OH)2 + 2HCl --> SrCL2 + 2H2O

p.s: My teacher said that once I determined the limiting reactant and found the excess, that the answer would become clear. However, I still cannot figure it out. Would someone please explain/show the steps on how to do this? Thanks a bunch.

You can not figure "it" out. Well if we knew what "it" meant, then perhaps we could help.
You can't figure out what the limiting reactant is?
You are clueless about determining what the relationship is between pH and [H(+)} and [OH(-)] ?
1. Set up chemical equation. Done.
2a. Calculate number of moles of HCl present
2b. Calculate number of moles of Sh(OH)2 present
3. Determine which is in excess
4a. If HCl is in excess, calculate pH from pH = -log([H+])
4b. If Sr(OH)2 is in excess, calculate [OH-] fro Ksp, then calculate pH from pOH.