A 25.0 mL sample of a 0.

I need some help with this problem; the problem asks about different amounts of ml of acid being added, but as long as I can do one, I can do rest on my own.

A 25.0 mL sample of a 0.1900 M  solution of aqueous trimethylamine is titrated with a 0.2375 M  solution of HCl. Calculate the pH of the solution after 10.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C.

Thanks.