NateG14 Posted February 21, 2007 Share Posted February 21, 2007 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. Link to comment Share on other sites More sharing options...
NateG14 Posted February 22, 2007 Author Share Posted February 22, 2007 Urgent help requested, please. Link to comment Share on other sites More sharing options...
John Cuthber Posted February 22, 2007 Share Posted February 22, 2007 Well you have got as far as the ratio of Na to acetate must be 1 to 1. What is that ratio now and what would you need to do to make it 1 to 1? Link to comment Share on other sites More sharing options...
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