In this problem, we are asked to find the pH of a mixture of acids.
Remember that HClO4 and HBr are strong, monoprotic oxyacid.
Recall that strong acids completely dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of HClO4 is as follows:
HClO4(aq) + H2O(l) → H3O+(aq) + ClO4–(aq)
The dissociation of HBr is as follows:
HBr(aq) + H2O(l) → H3O+(aq) + Br–(aq)
Find the pH of each mixture of acids.
1.5×10−2 M in HBr and 2.0×10−2 M in HClO4
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Gruet's class at Fresno City College.