posted by Niki on .
I don't know how to reply to an answer. First of all thank you!
For the question I just asked about the titration curves. Would that mean that titrating with barium hydroxide would take half the volume that is used when titrating with sodium hydroxide?
Oh and there was a second part to all of this...
If these two titrations were completed: 1) the titration of HCl with Na(OH) 2)the titration of acetic acid with Na(OH) (the concentrations of acid and base for both titrations are the same) How would the titration curves differ? Similar to before I know what the titration of the first one looks like but how would it be compared to the second one? Would the initial pH be higher/lower/same? Would the final pH be higher/lower/same?
Thank you a lot!
You reply to the response this way. When you read the response, scroll down and you will find a box below the response and that is where you put you next thoughts. We get some long threads that way on this board. First, for 0.1M HCl vs 0.1 M Ba(OH)2, it will take 1/2 the volume of Ba(OH)2 because it is 0.2M in hydroxide ion.
For acetic acid vs NaOH, the pH at the beginning is higher than for HCl. That's because HCl is a strong acid and ionizes 100% so the pH of a 0.1M soln of HCl is 1.0. For acetic acid that is 0.1M, that is a weak acid, the pH starts about 2.9. The equivalence point of the acetic acid/NaOH is not at 7.0 but about 8. The portion above the equivalence point is just excess NaOH so it looks about the same. Here are a bunch of sites that will show you how those look.