An aqueous solution of HBrO 4 has a pH of 4.34. Find the molar concentration of HBrO 4 solution.

Hey, guys. We're now going to answer the practice question that was left on the bottom of the page where we're asked to find the pH of H2SO4. 4. So, this question is different than the others. In this question, I give you ml's with the molarity. So, what exactly do we do with those liter, those milliliters? Well, you should realize here that we don't have to do anything with this volume. We would only use that volume if we were mixing this acid with a base. Here, I never made mention of another compound at all, so it's only a strong acid by itself. So again, you only would use that volume if you're mixing this compound with a base. Because we never make a mention of another compound. We don't with a strong acid by itself, so all we need to look at is the concentration. Also, we're going to say, remember, we may have 2 acidic H's and H2SO4 but that doesn't mean we multiply the concentration times 2. We're only on the lookout when it comes to strong bases. Because remember, in strong acids, the first stage that comes off is very acidic. But then the second one that's going to come off here is very weak. It doesn't really contribute to the concentration at all. It's okay to keep it as the same concentration. The question simply becomes pH equals negative log of that concentration. So equals 6.37. Hopefully, you guys were able to get this answer correct. If not, don't worry. It was kind of tricky. I didn't tell you exactly what to do with that volume.