🤓 Based on our data, we think this question is relevant for Professor Randles' class at UCF.
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.
A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?