anonymous
  • anonymous
Can anyone please help me with my lab report data? Desperate college freshman student looking for help with the topic of buffers.
Chemistry
chestercat
  • chestercat
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anonymous
  • anonymous
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haleyelizabeth2017
  • haleyelizabeth2017
I don't believe I know how to do this. What science is this?

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anonymous
  • anonymous
Chemistry, if you know anyone who can. Please let me know!
anonymous
  • anonymous
anonymous
  • anonymous
aaronq
  • aaronq
I'll take a look at it if you post it in a pdf format (rather than word)
anonymous
  • anonymous
okay
anonymous
  • anonymous
@aaronq - Here you go. If I am not on. Email is jdalloo97@gmail.com.
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aaronq
  • aaronq
you should stay on if you wanna work through it. I'm only going to tell you how to do it, but i'm not gonna do it for you.
anonymous
  • anonymous
Okay, sure. Whatever's best.
anonymous
  • anonymous
I need to know theoretical pH, also but I don't know how to do that. Finding the missing columns are the most important ones.
aaronq
  • aaronq
do you have other data regarding the composition of the buffers, or anything like that? there isn't enough information on these sheets to complete this
anonymous
  • anonymous
Sodium Acetate and Acetic Acid are the substances that I used.
aaronq
  • aaronq
Okay cool. For the theoretical pH, we can use the Henderson-Hasselbalch equation: \(\sf \large pH=pKa+log\dfrac{[A^-]}{[HA]}\) so we need to know the initial concentrations of the components (sodium acetate and acetic acid) and how much acid or base you added.
anonymous
  • anonymous
1.0 M for each solution, which was labeled on the Erlenmeyer flask for the lab.
anonymous
  • anonymous
Regarding the amount added, it should be on the pdf file.
aaronq
  • aaronq
Is the data one second for the first table? it doesnt seem like it. For the first table, beaker 1. you added equal amounts of Na acetate and acetic acid? how much acid did you add, at what concentration?
anonymous
  • anonymous
What do you mean?
anonymous
  • anonymous
I could send you a pic of my lab scanned....is that fine?
aaronq
  • aaronq
On the first table, where it says "beaker, solution, measured pH..", what are the amounts of everything that you used?
aaronq
  • aaronq
Lets just work with the data for the first line, "Beaker 1" where you used buffer A + HCl
anonymous
  • anonymous
Okay, so first I added 25 mL of Buffer Solution "A" into Beakers 1 +3. I added 25 mL of distilled water to beakers 2 +4. Moreover, I transfered 1.0 mL of 1 M HCl to beakers 1+2, and 1 mL NaOH to beakers 3+4. I measured the new pH after that was done.
aaronq
  • aaronq
Hm nothing on the concentrations of the buffer? or the volumes? i was working through it and can't go forth without those
anonymous
  • anonymous
No sir. That's why i am stuck.
anonymous
  • anonymous
the volumes of the buffers + additional total to 26 mL.
aaronq
  • aaronq
We could assume that they're equal (both at 0.5 M to add up to 1 M buffer), since the pH (4.41) is close to the pKa (4.75) and it could be off solely because of experimental error.
anonymous
  • anonymous
Okay sure. Would that work, or cause any error in the calculations?
aaronq
  • aaronq
Well it would be wrong if the concentrations of the components of the buffers are anything but 0.5 M each.
anonymous
  • anonymous
True.
aaronq
  • aaronq
I mean i can show you how to do it with 0.5 M and if you come across the actual concentrations you can just rework through it later?
anonymous
  • anonymous
That would be great. Anything that's close is good for me. I had a headache trying to figure this out all day.
aaronq
  • aaronq
okay cool. we need to make an ICE table to keep things organized. It stands for Initial, Change and Equilibrium (concentrations). The reaction is: \(NaCH_3COO^-+HCl\rightarrow NaCl+ CH_3COOH \) we're only interested in the concentrations of sodium acetate and acetic acid. \([NaCH_3COO^-]\) \([CH_3COOH]\) I C E Initially, we had 25 mL of \([NaCH_3COO^-]\)=0.5 M and \([CH_3COOH]\)=0.5 M we have: \(moles=Molarity*volume=0.5~M*0.025~L=0.0125~moles\) for each \([NaCH_3COO^-]\) \([CH_3COOH]\) I 0.0125 moles 0.0125 moles C E The "change" was adding acid, \(moles=1~M*0.001~L=0.001~moles \) \([NaCH_3COO^-]\) \([CH_3COOH]\) I 0.0125 moles 0.0125 moles C -0.001 +0.001 E this makes sense because you neutralized some base (sodium acetate and made the same amount of acetic acid) \([NaCH_3COO^-]\) \([CH_3COOH]\) I 0.0125 moles 0.0125 moles C -0.001 +0.001 E 0.0125 -0.001 0.0125+0.001 The volume doesnt matter because of the math \(\sf \large pH=4.75+log\dfrac{(0.0125 -0.001)}{(0.0125+0.001)}\) this is the theoretical pH.
anonymous
  • anonymous
I don't be mean to sound super rude or anything, but I have to go in a little while. I apologize for the inconvenience.
aaronq
  • aaronq
I posted each step individually of the table so you could see how i filled it in
anonymous
  • anonymous
Thank you :)
aaronq
  • aaronq
This is for the buffers. for the water just use: \(\huge \sf pH=-log[H^+]\)
aaronq
  • aaronq
where \([H^+]\) is the concentration of HCl (in the new volume)
aaronq
  • aaronq
no problem! let me know if you have questions
aaronq
  • aaronq
Also, for the \(\Delta pH\) column, (which means change in pH. you just find the difference (subtract) between the two measured pH's, before and after you added acid or base.
anonymous
  • anonymous
Sorry, to be a bother but I had a question about the concentrations of the acids and bases for the first table. Is that for the first step above.
aaronq
  • aaronq
hmm i'm not sure i understand which step you're referring to?
anonymous
  • anonymous
Where you displayed the ICE table, is that just for theoretical pH?
aaronq
  • aaronq
yeah, that's for the theoretical pH. for \(\Delta pH\) just find the differences between the measured pH values
anonymous
  • anonymous
and for the [acids] and [bases],, how would i follow from previously mentioned steps.
aaronq
  • aaronq
So were talking about the second table right?
anonymous
  • anonymous
Yes.
aaronq
  • aaronq
Okay, so for that we use the value you mentioned before 1.0 M for each of the components. So for A, we had 25 mL of each base and acid, that is sodium acetate and acetic acid. We need to find the moles of each and the new concentration (molarity). \(\sf moles_{Base}=1~M*0.025~L=0.025~moles\) \(\sf Molarity=\dfrac{0.025~moles}{0.025~L+0.025~L}=0.5~M\)
anonymous
  • anonymous
Thanks!
aaronq
  • aaronq
no problem!

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