Posted by Shelley on Wednesday, May 12, 2010 at 4:04pm.
Certainly I know what a titration is BUT I'm not familiar with a virtual titration experiment.
The molarity is calculated
Macid x mLacid = Mbase x mL base provided the reaction is 1:1 such as HCl and NaOH. It can't be done that way if the reaction is not 1:1 such as NaOH and H2SO4 or NaOH and H3PO4. I am assuming you would have started off with the simplest which is 1:1.
The answer comes out in molarity which is moles/L which would be the H^+ concn.
I need to know more about the acid/base combination in order to predict the indicator to use. For the amount of titrant to add, if you go too fast (1 mL) you overshoot the equivalence point and if you go too slow (0.05 mL which is about 1 drop) the experiment takes too long.
I found the sciencegeek page but I didn't find a link to a virtual titration. Sorry I couldn't be of more help.
The web site for sciencegeek -you need to type in Shockwave/Titration after sceiencegeek
So when I take the volume of base times the moles of base and divided by volume of acid, that gives me the [H+] of the acid, correct?
OK. I found the site and did one titration and obtained the right answer so I suppose I did it right. ;-). Here is what you do and I've added some comments at the end.
Select 0.05 M NaOH
Add 1.00 mL increments until the indicator changes color, write down the number of mL, then click on redo experiment. On the second try, add 1.00 mL increment until you get to 1 mL LESS THAN the first time, then click on 0.05 mL and add dropwise (0.05 mL) until the color changes, then mLbase x Mbase = mLacid x Macid and calculate M acid. Then you type that answer into the box on the right hand side and it tells you if you are right or not.
[notes:I didn't play around with the indicators and I didn't change acids (just A) so I don't know if they are 1:1 or not. My best guess is that they are simple titrations and that any indicator will work but that is just a guess. If you have trouble, post and I can go back and try it again. Also, my best guess is that acids A-E are always the same when one checks in; i.e., I get the same acids A-E when I try as you will get when you try but that's just my best guess. If my guess is right, then acid A is 0.06 M for H^+. P. S. the instructions are to type in the number only so .06 gets it without the M]
Thanks so much-I really appreciate it
OK. I've run A through E and all of them were correct. You will find that some of them, if you use 0.05 M, will not titrate with 50.0 mL (all the buret will hold) and it will be necessary to redo the titration using 0.1 M or 0.4 M. The obvious choice is to try 0.1 first and if that won't do it switch to 0.4 M NaOH. The procedure is always the same. Make one run clicking fast on 1 mL, restart, add to 1 mL less than what it took the first time, then switch to 0.05 mL (with the same sample), this time adding slow enough that you can stop when the color changes, then do the titration. You must be careful that the box to type in the answer shows the same letter as the acid you are titrating. Mine didn't always show that and I had to mess around with the arrows until I got the right letter in the box, then I typed in my answer. I always had the right answer so I don't know what the hint button does. One other note: I think it times out after 30 minutes and I had to start over, between looking at the site and coming back to Jiskha to give you instructions. Anyway, I hope this takes care of the problem.