Hello there ! First of all, thank you very much for the brilliant content. I'm a PhD in organic chemistry and watched your video on chlorine gas which helped me in the lab regarding the drying glassware (not kidding). Decided to scroll through your content and actually love to watch you manipulate these basic stuff which we usually just buy (Bromine, Iodine, etc...). Anyway love the way you show chemistry to the world, keep rocking ! ;)
You know what I would love to see? I want to see scrapings taken from the blades of your fan sent for a full assay to see what kind of crazy compounds have formed from all the traces on it reacting.
Infact, Iodine can easily exist as a fuming liquid at increased temperatures and atmospheric pressure. The fact that it can't is a common misconception.
I was able to produce liquid iodine at elevated temperatures and normal atmospheric pressure while trying to crystallize it onto a cold flask through sublimation. It wasn't hard at all.
*Elemental Maker* showed a neat trick in his iodine video where he submerged the powdered iodine (extracted from some medical product containing iodine, similar to this) in concentrated H2SO4, then heated it up until the iodine was liquid, then let it cool. Once cooled, he poured the H2SO4 off and the iodine came out as a solid little pellet, which was really shiny and pretty. Definitely something worth doing (gives less surface area, so less iodine sublimates, making it last much longer.
A classic method to make iodine :) I use sulfuric acid instead of HCl and sodium iodide, because those where cheaper for me. For resublimation I highly recommend adding ice to the round bottom flask. This gives very beautiful, pure, large iodine crystals :) Nice video!
Iodine can actually be liquid at atm pressure at around 110 deg C. It‘s just that it has such a high vapor pressure which causes most of it to sublime before reaching the liquid phase
The deal about iodine not having a liquid state at 1 atmosphere is a common misconception. Iodine WILL melt a little above 100C in an open beaker. In fact, it often happens when sublimbing iodine to purify it. The same is true of mothballs (either naphthalene or paradichlorobenzine). If you put some in a jar, cap with foil, invert, and place on (only slightly warm) hotplate, beautiful needle crystals will form on the sides of the jar. Depending on heat, mothballs may melt in the foil cap, but the crystal formation is sublimation. While mothballs in cap are liquid, shut off heat, lift jar off cap, and put "real" cap on jar, for a permanent crystal display! You could do this with iodine, but you would need some other material to replace the foil with that would not react with the iodine.
A pretty neat way to prepare dry iodine is to melt the iodine under conc. sulfuric acid, which results in one solid lump of iodine. The iodine lump traps a few drops of acid in it so at least a single sublimation should be performed to optain a pure product.
excellent video!! I love your Laboratory!! Building mine slowly.Did you take chemistry as a subject or did you just teach yourself? You know a lot about it!!
Doug's Lab, great work and thanks for sharing. I have 37% HCL how much of that should I use or how do I make it 25% before using it to make the crystals? thank you
Don't you lose most of the iodine in the solution due to its solubility of iodine in KI solution? Can you rig the reaction to use up all the KI and HI?
Solubility and time needed to dissolve are actually mostly unrelated. Solubility is a thermodynamic property but dissolution rate is a kinetic property.
How about you wash iodine with a water-miscible solvent in which iodine does not dissolve? It should suck all the moisture, shouldn't it? If the solvent is more volatile, it should vaporize quicker iodine.
How is your yield from starting amount of pottasium iodide? I saw many of your iodine left in filtrate solution, so is it because of remaining KI, that dissolves I2, or KCl ?
+pcworld The yield is only moderate. Most of the coloration in the filtrate is because it was filtered warm. There is excess HCl/H2O2 so there should not be any iodide left to solvate excessive iodine. I did not calculate the yield for that batch but if I weigh the container it comes to 84% over two runs. I'm sure this could be modified to get 95+% but KI is cheap for me so this is sort of a "quick-and-dirty" preparation.
+pcworld +Doug's Lab If you really wanna squeeze the yield to the maximum you should use a greater amount of H2O2 to oxidize more of the KI. Why? Iodine isn't really soluble in water (as Dough already mentioned) but iodine is highly soluble in aqueous KI (for more information: Lugol's Iodine). So if you reduce the remaining KI in solution you will increase the amount of iodine which precipitates out. After all you can extract the remaining iodine from the aqueous solution using EtOAc. Hope I was able to answere your question.
The radiation sickness thing only applies to the radiation from Iodine 131, and saturating the thyroid only works _before_ exposure. It'll offer basically no protection against modern nuclear waste or weapons. An extra serving of iodised table salt before the exposure would be more or less sufficient to protect against I131, though it's doing nothing to protect against all the other radioisotopes.
I could not understand what you were saying the HI was. Some sorts of Hyur..something acid. I listened four times and still couldn't make it out. Way too fast.
yes it does. As DOugh mentioned though this is nort the way to go if you need HI as HI is WAY stronger than HCl means the equilibrium is there but ist drastically on the left side. that´s what your oxidizing agent is for to constantly take out the forming HI as Iodine and prevent the backwards reaction. But yes HI is you conjugated Acid in this case. and you could without the H2O2 see for real, that the conjugated acid is an acid. you could see it´s color shortly ,but measuring the Ph you would get what you´d expect for a HCl solution of that concentration. SO for learning Acid and base reactions this reaction actually is quite useful, as you have visual evidence of the His presence while measuring that you only have an incredibly small amount of it.
@@BeastM140i If you take 7g iodine and 100 ml of water (ml, because the density of water is practically 1 g/ml) then you get less than 7% solution. To make 7% solution you have to take the whole solution's mass, not only that of solvent, so to make 7% solution of iodine you'd need 7g of iodine per 93g of water (ignoring the fact that it's impossible to dissolve that much iodine in water)
BigDog KMnO4 can be used to turn a alkene to a diol, so I imagine wherever there is a double bond in whatever molecule a bacteria or yeast has, an OH gets added to each carbon atom.
We're not allowed to have decent concentrations of hydrogen peroxide in England because our stupid government thinks we're going to use it to make bombs. You're so lucky in America or Canada because your government isn't as scared of chemicals as ours.
Hello there ! First of all, thank you very much for the brilliant content. I'm a PhD in organic chemistry and watched your video on chlorine gas which helped me in the lab regarding the drying glassware (not kidding). Decided to scroll through your content and actually love to watch you manipulate these basic stuff which we usually just buy (Bromine, Iodine, etc...).
Anyway love the way you show chemistry to the world, keep rocking ! ;)
You know what I would love to see? I want to see scrapings taken from the blades of your fan sent for a full assay to see what kind of crazy compounds have formed from all the traces on it reacting.
Infact, Iodine can easily exist as a fuming liquid at increased temperatures and atmospheric pressure.
The fact that it can't is a common misconception.
This is truth.
Yep, i was gonna comment this. NileRed did a vid on it
ruclips.net/video/dPIaEWd8zf4/видео.html
I was able to produce liquid iodine at elevated temperatures and normal atmospheric pressure while trying to crystallize it onto a cold flask through sublimation. It wasn't hard at all.
@@BackYardScience2000 Something tells me that this is church, y0. ;-) No, I do not have a sample of iodone...
@@TechGorilla1987 , well you will have a sample very soon. ;)
*Elemental Maker* showed a neat trick in his iodine video where he submerged the powdered iodine (extracted from some medical product containing iodine, similar to this) in concentrated H2SO4, then heated it up until the iodine was liquid, then let it cool. Once cooled, he poured the H2SO4 off and the iodine came out as a solid little pellet, which was really shiny and pretty. Definitely something worth doing (gives less surface area, so less iodine sublimates, making it last much longer.
A classic method to make iodine :) I use sulfuric acid instead of HCl and sodium iodide, because those where cheaper for me. For resublimation I highly recommend adding ice to the round bottom flask. This gives very beautiful, pure, large iodine crystals :) Nice video!
Iodine can actually be liquid at atm pressure at around 110 deg C. It‘s just that it has such a high vapor pressure which causes most of it to sublime before reaching the liquid phase
The deal about iodine not having a liquid state at 1 atmosphere is a common misconception. Iodine WILL melt a little above 100C in an open beaker. In fact, it often happens when sublimbing iodine to purify it.
The same is true of mothballs (either naphthalene or paradichlorobenzine). If you put some in a jar, cap with foil, invert, and place on (only slightly warm) hotplate, beautiful needle crystals will form on the sides of the jar. Depending on heat, mothballs may melt in the foil cap, but the crystal formation is sublimation. While mothballs in cap are liquid, shut off heat, lift jar off cap, and put "real" cap on jar, for a permanent crystal display! You could do this with iodine, but you would need some other material to replace the foil with that would not react with the iodine.
A pretty neat way to prepare dry iodine is to melt the iodine under conc. sulfuric acid, which results in one solid lump of iodine.
The iodine lump traps a few drops of acid in it so at least a single sublimation should be performed to optain a pure product.
excellent video!! I love your Laboratory!! Building mine slowly.Did you take chemistry as a subject or did you just teach yourself? You know a lot about it!!
Great video. But H2O2 will react with Cl- to form chlorine. Better reaction would be decomposition of silver iodide which happens without heating.
Thank you, Doug. You're a great chemistry teacher!🤗
You could dry the I by subliming it at about 40°C. The water wont evaporate but the iodine will. No loss of product.
Doug, for the love of everything, please put a piece of tubing on that aspirator outlet so it doesn't sound like a river :D
Does it make you want to pee?
Nah, it just sounds like a complete english breakfast being made
Hi , any chance you could do a short segment on your vaccuum setup , like how the aspirator is plumbed please ?
+Doug's Lab Why not store the iodine in the freezer instead of the fridge like you suggested with Br (to further lower the vapor pressure)?
I love you you explain the formula and the choices you have to achieve the reaction.
Been browsing through your videos for the past week, what a coincedence you chose to post now. Are you back for good? :)
this is a great video! i just referd back to use this and it was very helpful thanks!
Doug's Lab, great work and thanks for sharing. I have 37% HCL how much of that should I use or how do I make it 25% before using it to make the crystals? thank you
Great Video!!
Don't you lose most of the iodine in the solution due to its solubility of iodine in KI solution? Can you rig the reaction to use up all the KI and HI?
Solubility and time needed to dissolve are actually mostly unrelated. Solubility is a thermodynamic property but dissolution rate is a kinetic property.
That is a common misconception iodine does have a melting point
I was JUST gonna say that
Nah, he said "at atmospheric pressure", and he's right. At that pressure it sublimes.
It melts at 113.5C, boils at 184.35C, but also has a high vapor pressure.
Thor Correia no, you can melt in at atmosphere
I have also melted iodine into a liquid at normal atmospheric pressure. That myth has been proven false for some time now.
iodine does liquify when you heat it up ig goes to a liquid and than really fast to a gas
Hello Doug's Lab I was wondering what would be the purity percentage of the Iodine in the end.
I was wondering what your yield of bromine was because you did not mention it in the video?
could put a round bottom flask filled with ice water on top of the flask after adding H2O2 , that should help catch some of those iodine vapors.
I am curious about your vacuum system. How does it work?
You should record a tour of your lab so we can see how it's all set up. =)
+Erik The first video on this channel he gives a basic tour.
I love the smell of that stuff but I'm guessing it's pretty dangerous to inhale very much.
Hi, how many times do you have to rinse the crystals if you don't have a vaccum filter?
hey dough can u make a demonstration of the formation of fluorine?
using this method of extracting what is the purity of these iodine crystals?
What are prilled iodine crystals? I know the globules definition but any benefit or just industry standards?
Do you make and store other halogens?
HI is thermally unstable, so perhaps you don't even need the peroxide? Loss of H2 drives the equilibrium over, probably sped up by heating.
2KI also reacts with H2O2 to form I2 and 2KOH
No one can get a halogen heavier than Iodine. Can you make Astatine? or Tennessine?
how much hydrogen peroxide should I use instead of 25% concentration, as I do not have access to 25% but I do have access to 3%.
Wait wait... it's flourine(floureen), chlorine(chloreen), bromine(bromeen) and not iodine(iodeen)? Is Iodine(iodayn) valid?
Now all I need is a red phosphorus synthesis and I'll be making some money
mama miya i appreciate ur hardwork
what was your percent yeild ?
2:55 why are your gloves so stained?
How about you wash iodine with a water-miscible solvent in which iodine does not dissolve? It should suck all the moisture, shouldn't it? If the solvent is more volatile, it should vaporize quicker iodine.
Thats so awesome!!!!!!!!!! You should really make a video of what happens when you mix soda with mercury
No chemical reaction happens.
Could you use the pistol apparatus for this?
I think it's better to use sulfuric acid, as hydrogen peroxide in an acetic enviroment will react with chloride ions to produce chlorine
How is your yield from starting amount of pottasium iodide? I saw many of your iodine left in filtrate solution, so is it because of remaining KI, that dissolves I2, or KCl ?
+pcworld The yield is only moderate. Most of the coloration in the filtrate is because it was filtered warm. There is excess HCl/H2O2 so there should not be any iodide left to solvate excessive iodine. I did not calculate the yield for that batch but if I weigh the container it comes to 84% over two runs. I'm sure this could be modified to get 95+% but KI is cheap for me so this is sort of a "quick-and-dirty" preparation.
+pcworld +Doug's Lab
If you really wanna squeeze the yield to the maximum you should use a greater amount of H2O2 to oxidize more of the KI. Why? Iodine isn't really soluble in water (as Dough already mentioned) but iodine is highly soluble in aqueous KI (for more information: Lugol's Iodine). So if you reduce the remaining KI in solution you will increase the amount of iodine which precipitates out. After all you can extract the remaining iodine from the aqueous solution using EtOAc.
Hope I was able to answere your question.
is there a way to store it with out it disappearing or degrading .and is it good for radiation sickness .
The radiation sickness thing only applies to the radiation from Iodine 131, and saturating the thyroid only works _before_ exposure. It'll offer basically no protection against modern nuclear waste or weapons. An extra serving of iodised table salt before the exposure would be more or less sufficient to protect against I131, though it's doing nothing to protect against all the other radioisotopes.
could you please tell me what molar Hal u used
I could not understand what you were saying the HI was. Some sorts of Hyur..something acid. I listened four times and still couldn't make it out. Way too fast.
Hydroiodic acid.
Yes, I know I'm a couple years late but this might be useful for others
💜
In this reaction does the KI act as a base when reacting with the HCl and then form a conjugate acid (HI) & a conjugate base? (KCl)
yes it does. As DOugh mentioned though this is nort the way to go if you need HI as HI is WAY stronger than HCl means the equilibrium is there but ist drastically on the left side. that´s what your oxidizing agent is for to constantly take out the forming HI as Iodine and prevent the backwards reaction. But yes HI is you conjugated Acid in this case. and you could without the H2O2 see for real, that the conjugated acid is an acid. you could see it´s color shortly ,but measuring the Ph you would get what you´d expect for a HCl solution of that concentration. SO for learning Acid and base reactions this reaction actually is quite useful, as you have visual evidence of the His presence while measuring that you only have an incredibly small amount of it.
Are these the Iodine crystals I pack into wounds on my horses ? I was able to buy them at the feed store till they got to problematic to buy.........
+Me Craig Possibly, now they are strictly regulated due to use in drug production.
David Zed
....Say it aint so ! ........ Thanks ...... your videos are very interesting...Again Thanks
The good news is that KI is not regulated. The price has gone way up since that Fukushima disaster. The price on geiger counters is up as well.
banger title bestie
it totally does have a liquid state!
What was your return?
Is your vacuum pump powered by your sink?
In fact, yes. en.wikipedia.org/wiki/Aspirator_%28pump%29
12:59 = Doug's face in the flask
why not use NaI instead?
Melt some iodine down under sulfuric acid. Makes for a very nice sample for a collection.
What was your yield??
How do you make medical (liquid) iodine? Something from this?
Dissolve elemental Iodine in alcohol... the full medical name is "tincture of iodine"
Can you explain how to make a 7% tincture with that pretty powder?
Just use percentages. I assume it’s weight/weight? So it’s 7g iodine per 100ml of water
@@BeastM140i That would be rather 7 grams of iodine per 93 ml of water.
@@d113lll7 no that’s volume/volume. I went by weight/weight
@@BeastM140i If you take 7g iodine and 100 ml of water (ml, because the density of water is practically 1 g/ml) then you get less than 7% solution. To make 7% solution you have to take the whole solution's mass, not only that of solvent, so to make 7% solution of iodine you'd need 7g of iodine per 93g of water (ignoring the fact that it's impossible to dissolve that much iodine in water)
@@d113lll7 oh shit. You’re right. Sorry mate I’m horrendously tired.
Would 6% H2O2 work?
nice!
If you could please use subtitles that would be good thanks xxbridge
I remember using Ipermangonate as a kid for antiseptic
Potassium permanganate. It is a very strong oxidizing agent.
louis tournas which is why it works I guess.
BigDog
KMnO4 can be used to turn a alkene to a diol, so I imagine wherever there is a double bond in whatever molecule a bacteria or yeast has, an OH gets added to each carbon atom.
How much pure is the HI you did?
Sayeth the meth maker
+Thebarnardfactor Took the words right out of my mouth....
Science
make tour of your lab!!!
I guess I missed what percentage the peroxide was, I’m guessing 30 percent but I could be wrong
I've just realised that Doug could be a shortened version of the name Douglas...I'm almost 22 and haven't felt this ashamed in a while
NorthWest,ON,Kanada
Just quick note, iodide doesn’t sublimate. It have liquid form. Nice video.
Just because it has a liquid form, doesn't mean it doesn't sublimate. It can do both you know...
"sublimes"
Yeah man, it rocks out to those jams.
At 12:53 you can see his face in the reflection on the bottom left corner👀
0:00 - 2:01 YOU HURT MY BRAIN ,,,,,,
We're not allowed to have decent concentrations of hydrogen peroxide in England because our stupid government thinks we're going to use it to make bombs.
You're so lucky in America or Canada because your government isn't as scared of chemicals as ours.
Not much better in austria. Everything above 12% is illegal here... same for nitrate salts or nitric acid above 3%.
Drakkar Calethiel concentrate the peroxide by freezing, works great
Chem1456 can't do that 'cus if I do our glorious leader will send the KGB round to spank me.
aha
you can freeze the water in 12% the just drain off 35%
I keep mine in the freezer.
Why - SO?!.)
Why not in case: KJ + H3BO3 + MnO2 --> J2 + K2B4O7 + MnB4O7?;)
- or KJ + H3PO4 + MnO2 --> J2 + KH2PO4 + MnHPO4
2KI + H2O2 + H2SO4 → I2 + 2H2O + K2SO4
I believe the sulfuric acid will oxidize the iodine, but phosphoric acid or hydrochloric acid should work
u keft way too much unchanged. and didnnt wash the way you should
Messy.
Who can recommend me a book on synthetic organic chemistry?