Sigerson
Harmless
Posts: 14
Registered: 21-2-2014
Member Is Offline
Mood: Contending with the Texan Dark Age
|
|
LiL help with Solution Extraction
Greetings all,
This is my first post outside of the legal and societal forum so before I continue, please forgive me in advance if what I'm asking here is readily
available elsewhere. I did search to no avail so that said.....
I'm working through a few labs found in Bob Thompson's illustrated guide to chem. He has been amazingly kind and patient with me as I bombarded him
with myriad questions initially but I think it's time to return that favor and give him a break. And so, I turn to you fine folks.
In the lab on solvent extraction, I applied lighter fluid to a test tube filled with iodine solution (1.27% I and 1.67% KI) and water and sure
enough, in short time a deep purple layer formed along the top which I took to be the product layer.
My question really has to do with that layer. I moved it using a dropper to a petri dish to let it evaporate but come next day it just seemed to stain
the walls of the container around it yellow. I had it in a plastic bag just in case it tipped while in my drawer. Far as I can tell, it wasn't
disturbed but it did manage to turn everything inside yellow. Unfortunately, I'm guessing that's the iodine? There was still plenty of the purple
fluid in the dish which I then transferred to a dropper bottle. I have left the bottle open in hopes the fluid will evaporate as it still smells like
lighter fluid. Do I have any reason to keep the purple solution? If so why?
If it does evaporate, would I be left with pure iodine? If so, what happened to the potassium iodide? Again folks please forgive the simplicity of
these questions. This literally is my first foray into chemistry. I'm very excited but I want to understand as much as possible every step of the way.
Anyhow, I'll leave it at that for the time being. I really am so grateful for this forum and all of you. thank you in advance for your attention to my
questions.
P.S. a bit off topic I'm sure, but I understand I have to seek out permissions for certain chat rooms or forums? is this still true. Anyone in
particular I need to speak to?
Cheers. thanks all and good night
[Edited on 6-3-2014 by Sigerson]
[Edited on 6-3-2014 by Sigerson]
"Nothing has such power to broaden the mind as the ability to investigate systematically and truly all that comes under thy observation in life." -
Marcus Aurelius
|
|
|
Sigerson
Harmless
Posts: 14
Registered: 21-2-2014
Member Is Offline
Mood: Contending with the Texan Dark Age
|
|
Also, what would keep me from just adding more Lighter Fluid and extracting more out of the solution. I did it with two t. Tubes and they definitely
looked lighter when I was done with em but sill dark enough to indicate more iodine to extract?
"Nothing has such power to broaden the mind as the ability to investigate systematically and truly all that comes under thy observation in life." -
Marcus Aurelius
|
|
|
thesmug
Hazard to Others
Posts: 370
Registered: 17-1-2014
Location: Chicago, Il (USA)
Member Is Offline
Mood: No Mood
|
|
I have that book too! The yellow staining is from iodine, which tends to stain everything yellow. I don't think there's much use in keeping the purple
solution but yes, if you evaporate it I believe you will be left with pure iodine. The iodine will, however, sublime quickly and because of this you
might lose a lot of iodine, so be sure to pay attention to any purple vapor. If I'm understanding your question correctly the potassium iodide was
(assuming you're using HCl to produce said iodine) converted into potassium chloride, iodine and water, or hydroiodic acid and potassium chloride if
you didn't add the H2O2. The eq. for this reaction is: 2HCl + 2KI + H2O2 ---> I2 + 2KCl + 2H2O. I believe the permission-only forums require at
least 100 good posts (not being a jerk, not spamming etc...). Adding more lighter fluid wouldn't do much other than make a dilute solution if you have
already extracted all the water/KCl solution. I hope you have a good time doing all the experiments in that book!
[Edited on 3/6/14 by thesmug]
|
|
|
Mesa
Hazard to Others
Posts: 264
Registered: 2-7-2013
Member Is Offline
Mood: No Mood
|
|
What is reducing the KI to I2? Or are you only trying to extract the 1.27% of free iodine and leaving the KI in the aqueous layer? I'm not familiar
with the experiment myself, nor with the chemistry of Iodine salts in general, however it is interesting to me that I2 will migrate to an organic
solvent from an aqueous one so readily.
In any case, Iodine stains skin with a fairly obvious yellow tint, perhaps a similar reaction is occuring with something coating the walls of the
petri dish?
|
|
|
Metacelsus
International Hazard
Posts: 2539
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
The KI is most definitely left in the solution.
@Mesa: Iodine is more soluble in organic solvents than water (log Pow = 2.49)
The yellow color is due to staining from the iodine vapor.
|
|
|
Sigerson
Harmless
Posts: 14
Registered: 21-2-2014
Member Is Offline
Mood: Contending with the Texan Dark Age
|
|
Thanks for the replies all of you. Ill give a synopsis of the experiment. According to Bob Thompson's illustrated guide, lab 6:4, solvent extraction,
I filled one test tube half way with tap water. I then added 10ml of iodine solution. It says to use Lugols solution but I used an iodine solution I
assumed to be the same. It has 1.27 Iodine, and about 1.67 KI (potassium Iodide). I mixed this solution vigorously. I did this again in a second test
tube. so now with two test tubes mixed with iodine solution and water, in one of them I added 1ml of lighter fluid as my organic solvent, allowing it
to form a layer at the top of the aqueous solution. I repeated the process in the second test tube, this time using 5ml of lighter fluid. I mixed both
and eventually, a purple layer form at the top which I understand to be the product layer. I extracted the product layer and added it to a petri dish
and stored it in a plastic drawer. you're right, it eventually evaporate and turned everything yellow. Is that to say there's no iodine left after
everything evaporates? I put the remainder of the purple solution in a dropper bottle. Should I toss it then?
"Nothing has such power to broaden the mind as the ability to investigate systematically and truly all that comes under thy observation in life." -
Marcus Aurelius
|
|
|
thesmug
Hazard to Others
Posts: 370
Registered: 17-1-2014
Location: Chicago, Il (USA)
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by Sigerson  | | Thanks for the replies all of you. Ill give a synopsis of the experiment. According to Bob Thompson's illustrated guide, lab 6:4, solvent extraction,
I filled one test tube half way with tap water. I then added 10ml of iodine solution. It says to use Lugols solution but I used an iodine solution I
assumed to be the same. It has 1.27 Iodine, and about 1.67 KI (potassium Iodide). I mixed this solution vigorously. I did this again in a second test
tube. so now with two test tubes mixed with iodine solution and water, in one of them I added 1ml of lighter fluid as my organic solvent, allowing it
to form a layer at the top of the aqueous solution. I repeated the process in the second test tube, this time using 5ml of lighter fluid. I mixed both
and eventually, a purple layer form at the top which I understand to be the product layer. I extracted the product layer and added it to a petri dish
and stored it in a plastic drawer. you're right, it eventually evaporate and turned everything yellow. Is that to say there's no iodine left after
everything evaporates? I put the remainder of the purple solution in a dropper bottle. Should I toss it then? |
What you have is iodine water. If you wan't you can throw it away but I believe you can still use it for any application which would require iodine in
solution.
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
