I wasn't sure how to approach this problem, and I suppose the explanation makes sense to me, but I don't see why the answer utilizes the moles of HBr rather than the moles of KOH. Here's the question...
If 30ml of .02 M HBr solution is mixed with 40 ml of .03 M KOH, what is the pH of the mixture?
Edit: The only reason I can think of as to why the answer uses moles of HBr instead of KOH is because only the amount of the limiting reagent is utilized by the excess. But what confuses me is why pOH was derived from moles of acid over total volume. Is it because technically since KOH is in excess, we only use the amount of KOH as per what the limiting acid moles was? Sorry, I'm not wording this very well.
If 30ml of .02 M HBr solution is mixed with 40 ml of .03 M KOH, what is the pH of the mixture?
Edit: The only reason I can think of as to why the answer uses moles of HBr instead of KOH is because only the amount of the limiting reagent is utilized by the excess. But what confuses me is why pOH was derived from moles of acid over total volume. Is it because technically since KOH is in excess, we only use the amount of KOH as per what the limiting acid moles was? Sorry, I'm not wording this very well.