Sketch curve of pH vs volume of base added for the titration of 50.0ml of 1.00M acetic acid with 1.00M sodium hydroxide.
none, i think.
The Attempt at a Solution
Okay, first off, this is a weak acid, the first point on the curve would be the initial [H+] in the solution, so pH=-log([H+]). But i thought weak acids have very few H+ ions, almost none, thus the initial [H+]=0, but there is no exponent (other than infinity) that will give you zero, so this must be a situation where you use an ICE table to find [H+], but i was given no Ka value! so how can i solve for "x" in the ICE table? Can someone show me exactly how to find the important points so i can sketch the graph. thanks.
p.s. the pKa value of acetic acid was given in a previous question, i wonder if i am allowed to use it in this problem? I am really stuck here...