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.
http://www.google.com/search?q=titration+curves.&ie=utf-8&oe=utf-8&aq=t&rls=org.mozilla:en-US:official&client=firefox-a
You're welcome! I'm glad I could help.
To answer your first question about titrating with barium hydroxide (Ba(OH)2) compared to sodium hydroxide (NaOH), the volumes used would not necessarily be half. The volume required for a titration is determined by the stoichiometry of the reaction between the acid and base, not by the specific base being used. It depends on the balanced chemical equation and the molar ratios of the acid and base involved in the reaction. So, in general, you cannot assume the volume needed will be exactly half when using a different base like barium hydroxide.
Now, moving on to your second question about the titration curves:
1) In the titration of HCl with NaOH, HCl is a strong acid and NaOH is a strong base. The initial pH of the HCl solution will be very low (acidic) since HCl is a strong acid. As the NaOH is gradually added during titration, the pH will increase slowly until it reaches the equivalence point, where the moles of HCl and NaOH are in stoichiometric equivalence. At this point, the pH will be around 7 (neutral) because the solution contains NaCl, which is a neutral salt.
2) In the titration of acetic acid (CH3COOH) with NaOH, acetic acid is a weak acid and NaOH is still a strong base. The initial pH of the acetic acid solution will be higher than the initial pH of the HCl solution since acetic acid is a weak acid and therefore slightly acidic. As NaOH is added during titration, the pH will increase but at a slower rate compared to the titration of HCl. This is because acetic acid does not ionize completely, so there will still be some undissociated acetic acid present even at the equivalence point. Therefore, the final pH will be slightly higher (more basic) than 7 due to the presence of the conjugate base (acetate ion, CH3COO-) from the partial dissociation of acetic acid.
In summary, the initial pH of the acetic acid titration will be higher than that of the HCl titration, and the final pH of the acetic acid titration will be slightly higher than neutral (around 7), while the final pH of the HCl titration will be exactly neutral (pH = 7) due to the different strengths of the acids involved.
I hope this clarifies your questions! Let me know if there's anything else I can assist you with.