mole of the first one is M x L = 0.018075 which rounds to 0.0181 to three s.f.
mole of the second one is 0.0180726 which rounds to 0.0181 to three s.f.
So you are at the equivalence point of a strong acid/strong base so you have the salt (which is KClO4) and water. Therefore, the H^+ is determined by the ionization of water. The H^+ is 1 x 10^-7 M. The OH^- is 1 x 10^-7 M.
Hi! Thank you for your help...
A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 66.2 mL of KOH is ______M. (The answer is supposed to be 1.00X10^-7)
How do I set this problem up? I realize that it is a strong acid-strong base titration, but I don't know what to do..
thanks!!
1 answer
8 answers