We’re being asked to calculate the equilibrium constant of HA if a 0.10 M solution has a pH of 4.5
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of HNO2 is as follows:
HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq)
The pH of 0.10 M of an unknown acid is 4.5. Calculate the Ka of the acid.
a. 1.0 x 10-9
b. 1.0 x 10-8
c. 3.16 x 10-5
d. 1.0 x 10-10
e. 3.16 x 10-6
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 Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.