Question

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.

Related Questions

25 mL of a 0.10 M solution of the weak acid hydrofluoric acid, HF, (Ka = 7.2 x 10-4) is titrated wit... A 30.00 mL volume of a weak acid, HA, (Ka = 3.8 x 10^-6) is titrated with 39.00 mL of 0.0958 M NaOH... A solution of the weak acid HA was titrated with 0.100 M NaOH. the pH measured when vb=ve was 4.62 m... A sample of 0.314g of unknown monoprotic weak acid, HA was dissolved in 25.00 mL of water and titrat...