Problem: 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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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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Problem Details

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