posted by Patrick on .
A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0, 1, 5, 9, 9.9, 10, 10.1, and 12 mL.
This is done the same way I showed you for the NaOH/HBr titration (it would be nice if you didn't change screen names; it takes longer to get an answer when you do that) except that HA is a weak acid; therefore, when you find how much HA is in solution, you must set up an ICE chart to determine the (H^+) of the resulting HA solution and determine H from that. Everything else is the same.
Post your work if you get stuck.