Q: Find the pH during the titration of 20 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb = 5.2 x 10^-4), with 0.1000 M HCl solution after the following additions of titrant: (a) 0 mL; (b) 15 mL; (c) 20 mL; (d) 25 mL.
My Idea: I know that you need to find the excess moles for each addition of titrant. However, I do not know the equation of when the Base (CH3CH2)3N is added to the Acid (HCl). If I can get that, then I can obtain the moles of excess and figure out the concentrations for the Base and Conjugate Acid in order to get pH...
I don't mind if anyone wants to work this problem out and report to me your findings. I just need to find an equation to work with...Thanks for your time! I will award you for your time - the least i can do...
2007-04-02 17:32:55 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
The equation is a straightforward acid-base one, with a 1:1 mole ratio:
(CH3CH2)3N + HCl ----> (CH3CH2)3NH+Cl-
2007-04-03 01:29:35 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋