There is a titration of 5.00 mL .010 M NaOH with .005 M HCl. Indicate the pH of the initial and final solutions and the pH at the stoichiometric point. What volume of HCl has been added at the stoichiometric point

Question

There is a titration of 5.00 mL .010 M NaOH with .005 M HCl. Indicate the pH of the initial and final solutions and the pH at the stoichiometric point. What volume of HCl has been added at the stoichiometric point 
and the halfway point of the titration?

I have no idea how to solve this problem. I know that the stoichiometric point is always at 7 for strong acid-strong base reactions, but other than that I have no idea where to start.

DrBob222 · Answer

The stoichiometry point is when moles acid = moles base. moles base = M x L = ? moles acid = moles base moles acid = M x L. You know moles and M, solve for L and convert to mL.