We’re being asked to calculate the equilibrium constant of HPAc if a 0.12 M solution has a pH of 2.62
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of HPAc is as follows:
HPAc(aq) + H2O(l) ⇌ H3O+(aq) + PAc–(aq)
Phenylacetic acid (HPAc) is a modified form of an amino acid phenyl alanine seen in patients with phenylketonuria, an inherited disorder. A study of HPAc shows that the pH of a 0.12 M HPAc solution is 2.62. What is the Ka of HPAc?
A. 2.4 × 10–3
B. 4.8 × 10–5
C. 3.6 × 10–8
D. 5.0 × 10–4
E. 1.2 × 10–5
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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 Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.
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Based on our data, we think this problem is relevant for Professor Bartoszek Loza's class at OSU.