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anonymous
 one year ago
Can anyone please help me with my lab report data? Desperate college freshman student looking for help with the topic of buffers.
anonymous
 one year ago
Can anyone please help me with my lab report data? Desperate college freshman student looking for help with the topic of buffers.

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@acxbox22 @andrewjordan833 @alurahenderson @badmood @chycora @cupcakerain @desiringeden @desiraem @ElonaSushchik @freckles @GeniousCreation @haleyelizabeth2017 @HackberryAbby18 @ikram002p @JoKeR0331 @khalilforthewin @Lady.Liv1776 @mathmate @Nnesha

haleyelizabeth2017
 one year ago
Best ResponseYou've already chosen the best response.0I don't believe I know how to do this. What science is this?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Chemistry, if you know anyone who can. Please let me know!

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@alurahenderson @background43 @jadaaaa

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@abbi5169 @Brandonsnider222

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2I'll take a look at it if you post it in a pdf format (rather than word)

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@aaronq  Here you go. If I am not on. Email is jdalloo97@gmail.com.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2you 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
 one year ago
Best ResponseYou've already chosen the best response.0Okay, sure. Whatever's best.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I 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
 one year ago
Best ResponseYou've already chosen the best response.2do 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
 one year ago
Best ResponseYou've already chosen the best response.0Sodium Acetate and Acetic Acid are the substances that I used.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2Okay cool. For the theoretical pH, we can use the HendersonHasselbalch 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
 one year ago
Best ResponseYou've already chosen the best response.01.0 M for each solution, which was labeled on the Erlenmeyer flask for the lab.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Regarding the amount added, it should be on the pdf file.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2Is 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
 one year ago
Best ResponseYou've already chosen the best response.0I could send you a pic of my lab scanned....is that fine?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2On the first table, where it says "beaker, solution, measured pH..", what are the amounts of everything that you used?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2Lets just work with the data for the first line, "Beaker 1" where you used buffer A + HCl

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Okay, 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
 one year ago
Best ResponseYou've already chosen the best response.2Hm nothing on the concentrations of the buffer? or the volumes? i was working through it and can't go forth without those

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0No sir. That's why i am stuck.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0the volumes of the buffers + additional total to 26 mL.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2We 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
 one year ago
Best ResponseYou've already chosen the best response.0Okay sure. Would that work, or cause any error in the calculations?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2Well it would be wrong if the concentrations of the components of the buffers are anything but 0.5 M each.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2I 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
 one year ago
Best ResponseYou've already chosen the best response.0That would be great. Anything that's close is good for me. I had a headache trying to figure this out all day.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2okay 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
 one year ago
Best ResponseYou've already chosen the best response.0I 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
 one year ago
Best ResponseYou've already chosen the best response.2I posted each step individually of the table so you could see how i filled it in

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2This is for the buffers. for the water just use: \(\huge \sf pH=log[H^+]\)

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2where \([H^+]\) is the concentration of HCl (in the new volume)

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2no problem! let me know if you have questions

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2Also, 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
 one year ago
Best ResponseYou've already chosen the best response.0Sorry, 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
 one year ago
Best ResponseYou've already chosen the best response.2hmm i'm not sure i understand which step you're referring to?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Where you displayed the ICE table, is that just for theoretical pH?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2yeah, that's for the theoretical pH. for \(\Delta pH\) just find the differences between the measured pH values

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0and for the [acids] and [bases],, how would i follow from previously mentioned steps.

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2So were talking about the second table right?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.2Okay, 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). \(\sf moles_{Base}=1~M*0.025~L=0.025~moles\) \(\sf Molarity=\dfrac{0.025~moles}{0.025~L+0.025~L}=0.5~M\)
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