AP Chem student here with some trouble with A/B equilibrium. The problem and what I have done so far given below:
1. A solution contains .300 mol of acetic acid and .200 mol of sodium acetate in a total volume of 500 mL. How much 6.0 M NaOH must be added so that the pH of the solution equals the pKa of acetic acid? (Ka of acetic acid = 1.8 * 10^-5)
I apologize for not putting this in LaTeX, but the formula I must use, known as the Henderson-Hasselbach equation, goes as such:
pH = pKa + log([A-]/[HA])
where [HA] = the concentration (M) of the (weak) acid in question and [A-] = the concentration of the conjugate base. I understand that the ratio of
[A-]:[HA] must equal 1, as log(1) equals 0, and hence pH = pKa. However, given that the concentration of acetic acid is .6 M, and the concentration of the conjugate base (acetate ion) is .4 M, I do not understand how to calculate the volume of NaOH to be added without making the calculations unduly complicated. Assistance would be greatly appreciated.
P.S. I realized too late that this must go in the Homework Help forum. I would be thankful for a mod to move the thread if the rules require.
