I have been working on this problem for quite some time and was hoping that someone might have some suggestions on how to solve it:

"Calculate the pH of the final solution obtained after 200mL of 0.1 M NaOH is added to 300mL of 0.2 M H_{2}SO_{4}."

(H_{2}SO_{4} + NaOH --> Na^{+} + HSO_{4}^{-} + HOH)

I started working the problem by obtaining the total moles of salt that was created (which came out to 0.06 moles). I then figured out the total moles of NaOH to be 0.02 moles (which is also the amount of salt created--limiting reactant).

I am not sure where to go from here, should I use the Henderson-Hasselhoff equation?? Or am I on the wrong train of thought because this reaction contains both a strong acid and base? The pK value for Sulfuric Acid is also confusing me, because it's a strong acid different references give me different values (-3.00, -4.80, etc).

~~I tried plugging in the numbers into the HH equation but I come up with a negative pH, which I am sure is incorrect.

Any suggestions would be much appreciated, thanks!