We’re being asked to determine the pH of a solution when 31.0 mL of 0.125 M HClO4 is mixed with 25.00 mL of 20.0-mL of 0.150 M KOH
Let’s first write the balanced reaction between HCl and KOH:
▪ HClO4 → strong binary acid
▪ KOH → (OH- with Group 1A ion) → strong base
▪ the reaction between a strong base and strong acid → no need to create an ICE chart
Balanced reaction: HClO4(aq) + KOH(aq) → H2O(l) + KClO4(aq)
Now let’s find the concentration of reactant remaining after the reaction:
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added.
31.0 mL of the acid
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 Strong Base Titrations concept. You can view video lessons to learn Strong Acid Strong Base Titrations. Or if you need more Strong Acid Strong Base Titrations practice, you can also practice Strong Acid Strong Base Titrations practice problems.
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Based on our data, we think this problem is relevant for Professor MacFarland's class at CSU.