Problem: A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

FREE Expert Solution

We’re being asked to calculate the pH of a 1.25 M aqueous solution of Weak acid.

Weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). The dissociation of the generic weak acid HA is as follows: 


HA(aq) + H2O(l)  H3O+(aq) + A(aq)


From this, we can construct an ICE table. Remember that liquids are ignored in the ICE table.


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A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

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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 Randles' class at UCF.