|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
06-20-02 20:36
No 323416
|
|
|
|
Iodine
(Tincture) FAQ
|
Bookmark
Reply
|
|
|
I need someone to write an Iodine tincture FAQ, as I have very little on that
subject on my page, and everybody and their uncle are asking me about it in
PM and email...
Suggested Contents:
* All common oxidizers which can oxidize iodide to iodine + Reaction schemes
(and warn people of adding BOTH bleach and peroxide to the same solution as
some people seems to do, chlorine gas may be produced, and possibly other
nasty things).
* A list of the types of tinctures available (aqueous, alcoholic, 1%, 10%,
lugol's solution etc), and the best way of dealing with each of them.
* Typical yields.
* Storage, purification and drying of iodine.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-21-02 11:45
No 323606
|
|
|
|
Since
nobody writes here anything useful,i try to
|
Bookmark
Reply
|
|
|
Since nobody writes here anything useful,i try to come up with something.
Oxidisers used with tinctures:H2O2,NaOCl
Reactions shemes:
With H2O2: 2KI+2HCl+H2O2-->I2+2KCl+2H2O
With NaOCl:NaOCl+2HCl+2KI-->NaCl+2KCl+H2O+I2
Some of of H2O2 or NaOCl is used to form I2 from iodide:
2I+H2O2+2HCl-->I2+2H2O+Cl2
2I+NaOCl+2HCl-->I2+NaCl+H20+Cl2
NaCl and KCl go to water that is added before reaction.
Tinctures contain equal amounts of iodine salt and iodide
Tinctures:
1%-Not worth trying
2%-Shitty one but will do.
5%-Getting better
7%-Good for extracting
12%-Real gold for Swims,usually not available in stores and pharmacies,need
licence to get that.
Theoretical yield of I2 from KI is ~76 % and theoretical yeild of I2 from I
is 100%.
Iodine sublimes within few days when left on table.Also direct sunlight helps
subliming.Must be kept in closed container and in dark.Good way to dry iodine
is to lay it on newspaper or on toilet paper.Paper will suck liquid out
iodine.When iodine is really wet then one must change paper few times.
Dealing with tinctures:
Ratio of H2O2/KI is 2 moles of H2O2 per 4 moles of KI teoretically.Also we
need H2O2 to oxidise I to I2,that's 2 moles of H2O2 per 4 moles of
iodine.Ratio of KI/H2O2 is 68 grams of H2O2 per 664 grams of I2.Since KI/I
ratio in tincture is 50/50 we must use H2O2 to oxidise I too.That would be 2
moles of H2O2 per 4 moles of I.Thats 68 grams H2O2 per 508 grams of I.
Dream:
We have 2% tincture.
1 gram of KI and 1 gram of I.H2O2 needed is then 0,133 + 0,1=0,233 grams of
H2O2.Since we use 3% H2O2 then we would need 7,689 grams of 3% H2O2 per 100
grams of 2% percent tincture.
Now with 7% percent we must use 3,5 as much as with 2% so that's 26,9115
grams per 100 gram of tincture.
That's so only in theory.
Practically i use 2 times as much H2O2 as in theory to ensure
fast and full conversion.
OK Rhodium please check if formulas and calculations here are right and if
they are,i may add some calculations with NaOCl too.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
06-21-02 14:58
No 323629
|
|
|
|
Good
start!
|
Bookmark
Reply
|
|
|
There is a consistent molar ratio of I2 to KI in all the
commercial tinctures? Much easier to calculate with.
Your first scheme (with peroxide) is a bit off, you can divide all the
figures with 2, and also separating the reaction in two steps, first the
acidification and next the oxidation makes it easier to follow:
2 KI + 2 HCl -> 2 HI + 2 KCl
2 HI + H2O2 -> I2 + 2 H2O
Your rating of the different tincture strenghths, is that due to the lower
concentrations not being cost-effective, or is it hard to isolate the formed
iodine from such a large amount of water? The aqueous solubility of Iodine
only 300mg per liter, but if there is alcohol in the tincture, the solubility
will of course increase.
Is there more or less alcohol in different brands? Are there any alcohol-free
tinctures sold? What is the typical alcohol percentage in the solutions?
Theoretical
yield of I2 from KI is ~76 % and theoretical yeild of I2
from I is 100%.
With this you are referring to the non-scientific term "weight
yield", right?
I was more like wondering how much iodine you actually isolate in the end,
not how much is theoretically possible - that should be obvious to anyone who
bothers to calculate the molar weights.
When the manufacturers say "7% iodine", are they referring to 70g
of KI+I2 per kilo of tincture, or to the iodine/iodide alone
(meaning there is 77.2g KI+I2 per kilo of tincture?) Or is it per
liter of solution (I guess the density of the tincture isn't exactly
1.0)?
Other than just the math, the procedure is simply to mix the oxidizer with
the tincture and directly filtering off the iodine? Should the solution be
chilled first? Any special events happening using either oxidant? Any
concentration of peroxide works just as good?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-21-02 15:29
No 323639
|
|
|
|
So
many questions... Let's start with tincture.
|
Bookmark
Reply
|
|
|
So many questions...
Let's start with tincture.
They x% means obviously weight percent of I2+Iodine salt in tincture.Usually
it's 50/50 but may differ a little.And reason not to use low % tinctures is
that there is so much solvent around good stuff that it doesn't want to come
out.Most if not all of the liquid in tincture is alcohol and alcohol
dissolves I2.When one extracts 7% tincture he adds water to tincture so iodine
won't be so easily dissolved again innit.But some still dissolves and will be
thrown away.When using 7% the amount that dissolves again is small and it
won't affect yield that much but when using 2% then some of it dissolves
again in alcohol and will be thrown away .So yields are considerably lower
when dealing 2% compared to 7%.Also,i think,2% doesn't cost 3,5 times less
than 7%.2% percent tincture probably contains some water too but >5%
doesn't.Swim's tincture contains 2,5 percent of KI,2,5 percent of I and 0,2
percent of water and rest is alcohol.
Usually yields are over >80% with 5%(depends how careful one is when it
comes to drying)..Density of tincture should be near 1(Alcohol is ~0,8 gr/cm3
and Iodine is near 5.0 gm/cm3,but since there is lots of 0,8 gm/cm3 alcohol
and little 5.0 gr/cm3 iodine,the overall density is near 1).
Procedure itself is simple,yes,just mix oxidiser with tincture and them add
water and acid.Way too much oxidiser leaves one with iodine+some
crapola(over-oxidized iodine??)
that is hard to separate.
P.S i'll correct that reaction formula too.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
06-21-02 16:06
No 323647
|
|
|
|
Hasn't
anyone tried to concentrate the tinctures ...
|
Bookmark
Reply
|
|
|
Hasn't anyone tried to concentrate the tinctures by distillation? That should
leave only KI/I2, regardless of what concentration you started with.
Also, if using a weak tincture, after the oxidation step, the formed I2 could
be extracted with ether/chloroform/DCM, and especially if a concentrated salt
solution is added to the tincture to force out the alcohol from the aqueous
layer.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-21-02 16:35
No 323653
|
|
|
|
Distillantion-I'm
not so sure if it works.
|
Bookmark
Reply
|
|
|
Distillantion-I'm not so sure if it works.Iodine would sublime for sure and
get to recieving flask along with alochol.
Anyway you have something to start Iodine FAQ.Sure,i you have some
question,i'd be glad to help.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
06-22-02 09:37
No 323955
|
|
|
|
A
good procedure for iodate
|
Bookmark
Reply
|
|
|
A good procedure for reducing potassium iodate/sodium iodiate (KIO3/NaIO3)
might be helpful. Then we can reclaim all of that wasted iodide.
Edit: Hypoiodide (KOI/NaOI) reduction
would be appreciated also.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-22-02 10:03
No 323965
|
|
|
|
KIO3/NaIO3...really
don't know if one can use ...
|
Bookmark
Reply
|
|
|
KIO3/NaIO3...really don't know if one can use reducing agents with them.Maybe
hydrogen but really don't know if it works,althought KIO3 and NaIO3 should
give oxygen away easily.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
06-22-02 10:18
No 323970
|
|
|
|
Hypoiodide
|
Bookmark
Reply
|
|
|
former_chemist: KI + KOI + 2 HCl -> I2 + 2 KCl + H2O
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
06-22-02 10:18
No 323971
|
|
|
|
Strong
oxidizers
|
Bookmark
Reply
|
|
|
They (-IO3 compounds) are strong oxidizers. The Hypoiodous acid
salts (-IO) are harder to reduce. My current thought is direct reaction with
chlorine gas. All of the iodide should be replaced. Not particularly
safe but chlorine gas is not a lot more dangerous than hydrogen chloride.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
06-22-02 10:24
No 323973
|
|
|
|
Thanks
chief!!! former_chemist: KI + KOI + 2 HCl ...
|
Bookmark
Reply
|
|
|
Thanks chief!!!
former_chemist: KI + KOI + 2 HCl -> I2 + 2 KCl + H2O
Do you have one for the iodate, other than chlorine?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-22-02 10:46
No 323979
|
|
|
|
KIO3+3H2-->KI+3H2O
should be possible.
|
Bookmark
Reply
|
|
|
KIO3+3H2-->KI+3H2O should be possible but may be impractical.What do you
mean about direct reaction of KIO3 with
chlorine?6KI+KIO3+6HCl-->6KCl+KI+3H2O+3I2 should work fine too,like
KIO3 is oxidiser instead of H2O2 or NaOCl.Haven't tried but teoretically
should work
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
06-22-02 12:05
No 323985
|
|
|
|
Direct
reaction with chlorine
|
Bookmark
Reply
|
|
|
Inorganic iodide salts can be reacted with chlorine gas to yeild
iodine. This method is very old. It is one of the early methods
of extracting iodine from seaweed residue. This is done in a dry
environment because in water chlorine gas and iodide produce Iodic acid and
hydrochloric acid.
Sodium Bisulfite will reduce the Iodate Salt to Iodine and a salt
sulfate. Sulphur Dioxide will reduce Iodic acid to Iodine and sulphuric
acid. Sulphur Dioxide will reduce the iodate salts yeilding iodine and
sulphates. Heating iodate salts will release oxygen and either sublime
the iodide or leave a metal salt of iodine.
A little research goes a long way
http://33.1911encyclopedia.org/I/IO/IODINE.htm
It is obviously a scanned encyclopedia with little or no correction after
OCR.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-22-02 12:23
No 323988
|
|
|
|
Intresting...althougth
i think very few use it.
|
Bookmark
Reply
|
|
|
Intresting...althougth i think very few use it.It's for extracting iodine
from chile saltpeter or from seaweed.Most of swims stick to tincture.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
PrimoPyro
(Hive Prodigy)
06-22-02 16:55
No 324016
|
|
|
|
Iodates
|
Bookmark
Reply
|
|
|
Iodates react the same way hypoiodites do with iodide salts, precipitating
diatomic iodine, but more iodide must be used per iodate.
KIO3 + 5KI + 6HCl --> 6KCl + 3I2 + 3H2O
Hydrogen iodide is a powerful enough reducing agent to reduce iodate ions.
Don't forget that hypohalite ions give halate ions and halides upon strong
heating.
3MOX ==delta==> MXO3 + 2MX
PrimoPyro
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Elementary
(Hive Addict)
06-22-02 17:17
No 324020
|
|
|
|
Tinctures
with different %
|
Bookmark
Reply
|
|
|
While looking through the hive archives you will see many different
extractions methods, some maybe for 2%,4%,7% or even higher.
If you find a procedure for say 4% and you have 2% all you have to do is
evapourate half of the volume away to double the percentage in the tincture.
Just place you 2% tincture in a graduated beaker and sit it in a saucepan
with simmering water in it, as soon as the volume of tincture has reduced by
half, cool it in cold water, and you will have 4% tincture.
This same principle can be used to obtain 7% tincture from say 2%
John
Lennon - Working Class Hero
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
biojammer
(Stranger)
06-22-02 22:01
No 324104
|
|
|
|
no,
iodine sublimes!
|
Bookmark
Reply
|
|
|
read the earlier posts. i'm thinking that a copper colmn and stark trap for
the alcohol might work, recieving iodone in a condenser. but i don't really
know i don't do iodine.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-22-02 22:35
No 324114
|
|
|
|
Low
percent tinctures make extracting hard but ...
|
Bookmark
Reply
|
|
|
Low percent tinctures make extracting hard but one just might get LG iodine
if he searches really hard.LG isn't impossible to acquire and we still find
>5% tinctures.Only practical and effective method is still that oxidation
with H2O2 or NaOCl.IMO
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
fierceness
(Hive Bee)
06-23-02 03:06
No 324229
|
|
|
|
yes,
iodine sublimes, but does KI sublime?
|
Bookmark
Reply
|
|
|
yes, iodine sublimes, but does KI sublime? I didn't think KI would
sublime especially if it is in solution, but I could be wrong ;)
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-23-02 09:25
No 324332
|
|
|
|
KI
probably decomposed and then sublimes.
|
Bookmark
Reply
|
|
|
KI probably decomposed and then sublimes.If it doesn't decompose in solution
then how it could disinfect?Solution needs I ions to be disinfect
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
foxy2
(Distinctive Doe)
06-23-02 11:00
No 324344
|
|
|
|
ok
|
Bookmark
Reply
|
|
|
KI dissociates in solution(aqueaous) as do all salts of strong acids.
Thats what happens when salt dissolves, this has nothing to do with
sublimation and is not related. In general it is not possible to
sublime salts.
You can't sublime KI, it will melt first at 681C and then boil at 1330C.
Those
who give up essential liberties for temporary safety deserve neither liberty
nor safety
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-23-02 11:43
No 324350
|
|
|
|
Yep,i
was wrong.
|
Bookmark
Reply
|
|
|
Yep,i was wrong.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Elementary
(Hive Addict)
06-24-02 00:42
No 324484
|
|
|
|
Sublimation
|
Bookmark
Reply
|
|
|
I remember seeing one iodine extraction procedure from tincture, where the
first step was the evapouration of the ethanol.
I really don't beleive that there will be much sublimation by just
evapourating half of the ethanol.
See thread starting with Elementary: "Removing Ethanol from Tincture"
(Chemistry Discourse)
It all depends on how you look at the tincture :
1. An alcoholic solution of KI3.H2O
2. An alcoholic solution of KI and I2 and water
Most tinctures have a certain amount of water in them as well as ethanol, so
as long as there is water, there will be KI3. Potassium tri-iodide
only exists as the hydrate (KI3.H2O)
John
Lennon - Working Class Hero
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Elementary
(Hive Addict)
06-24-02 01:05
No 324489
|
|
|
|
It
could be possible to use liquid parrafin in ...
|
Bookmark
Reply
|
|
|
It could be possible to use liquid parrafin in the aid of extraction.
http://www.uwcsea.edu.sg/chem/IBfolder/IBH/PRACTICAL/Assessment/Examples/PlanA.htm
Here's my theory :
Buy floating a layer of liquid parrafin over the top of a
water,ethanol,iodine,potassium iodide mix. Upon heating the ethanol would be
the first to make the transition through the parrafin to the air.
Here some good info on tinctures:
http://thetillery.bizland.com/TinctureIodine.html
John
Lennon - Working Class Hero
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
06-24-02 01:29
No 324497
|
|
|
|
Can
somebody confirm that distillation of weak ...
|
Bookmark
Reply
|
|
|
Can somebody confirm that distillation of weak tincture is possible without
any sublimation or other problems occur?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
PrimoPyro
(Hive Prodigy)
06-24-02 02:31
No 324514
|
|
|
|
In
the past
|
Bookmark
Reply
|
|
|
I have attempted to isolate "iodine" from tincture bottles (this
was years ago when I did not know they contained KI) by evaporation of the
ethanol.
I boiled it to near dryness, and I never was able to recover any crystals,
only purplish film lining the walls of the container as the surface line
descended. I did not add anything to the tincture though, just started
heating a small bottle's worth until it got dry. Waste of time and money.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
tranceport
(Stranger)
06-24-02 07:34
No 324638
|
|
|
|
Is
iodine
|
Bookmark
Reply
|
|
|
Is iodine even that hard to get? I cant imagine it so...
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
weedar
(Hive Bee)
06-24-02 12:21
No 324723
|
|
|
|
Not
difficult to obtain..
|
Bookmark
Reply
|
|
|
I think the problem is getting a CHEAP source of iodine,
which tincture isn't..
Weedar
Weedar
contains 2,4-D dimethylamine salt,apparently
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
raffike
(Hive Bee)
06-24-02 12:39
No 324731
|
|
|
|
I
don't think iodine and rp would cause much ...
|
Bookmark
Reply
|
|
|
I don't think iodine and rp would cause much trouble,that's effy they are
asking huge price for.Anyway,this is a iodine thread so let's not argue about
other.Lab grade iodine is easy to get via college labs or some company.
A
friend with speed is a friend indeed
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
06-26-02 09:31
No 325531
|
|
|
|
Using
Sulphuric in place of HCl
|
Bookmark
Reply
|
|
|
Somewhere someone suggested using Sulphuric Acid in place of HCl in
converting KI in tinctures to HI. Your Rhodium: "Hydriodic Acid From Pinene and Iodine
" (Methods Discourse) explains why this is a bad idea.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Prepuce
(Newbee)
06-30-02 06:44
No 327054
|
|
|
|
H2SO4
vs HCl a bad idea to get I3 from tincture?
|
Bookmark
Reply
|
|
|
FormerChemist, you wrote:
"Somewhere someone suggested using Sulphuric Acid in place of HCl in
converting KI in tinctures to HI. Your Post No 288929 explains why this
is a bad idea."
But the title of that thread is "Hydriodic Acid From Pinene and
Iodine." I don't see any reference to extraction of I2 from tincture.
Was that the wrong link? Since SWIM uses H2SO4 / bleach (it's much easier, he
says) he'd really like to know what you intended to say.
Thanks,
PP
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
06-30-02 09:32
No 327091
|
|
|
|
From
Post 288929 : Re: My invention relates to a ...
|
Bookmark
Reply
|
|
|
From Rhodium: "Hydriodic Acid From Pinene and Iodine
" (Methods Discourse):
My invention relates to a new and improved process for the preparation of
hydriodic acid, either as the pure dry gas or as the aqueous solution. As is
well known, hydriodic acid can not be made satisfactorily by treating an
iodide with sulfuric acid as in the case of the preparation of hydrochloric
acid from a chloride and sulfuric acid. This is on account of the powerful
reducing properties of the acid. Thus, when an iodide, for example, potassium
iodide, is treated with sulfuric acid, some hydriodic acid is liberated but
in addition to the acid some iodine is set free. At the same time hydriodic
acid, on account of its powerful reducing power, reacts with the sulfuric
acid changing some of it to sulfurous acid and some to hydrogen sulfide. As
a result of this reduction, the yield of hydriodic acid is very small and the
acid is very impure. The preparation of hydriodic acid must therefore, be
other than the analogous method for the preparation of hydrofluoric or
hydrochloric acids.
The reaction described is what happens in converting the KI portion of
tincture using sulphuric acid. With HCl or phosphoric acid there is no reduction
of the sulphuric. Any chlorine gas formed when the bleach is added reacts
first with unreacted KI to form KCl and iodine. All this means is that when
using sulfuric your end yield will be less than when using HCl or phosphoric
acid. When reducing sulphuric more iodine is oxidized to HIO3.
Also note that hydrogen sulfide gas is formed which is more toxic than
chlorine gas.
Using sulfuric acid is equivalent to using too much bleach. That means
less iodine.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Hansje
(Hive Bee)
07-03-02 12:24
No 328276
|
|
|
|
bisulfite
is useful
|
Bookmark
Reply
|
|
|
Let me confirm (from practical experience) that bisulfite reduction of iodate
ion works very well. You have to add the bisulfite very careful, because too
much will also reduce your iodine to iodide.
Same warning goes for hypochlorite oxidation of iodide: too much will oxidise
your iodine to iodate.
(and then you can add bisulfite again to go back and forth through all these
pretty color changes for ever).
I think a warning is in place about adding either hypochlorite or bisufite to
strongly acidic mixtures (big clouds of poisonous Cl2/SO2 could form).
Hansje high in proteine and fibre!
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Osmium
(Stoni's sexual toy)
07-11-02 15:35
No 331262
|
|
|
|
When
you have a tincture which contains lots of ...
|
Bookmark
Reply
|
|
|
When you have a tincture which contains lots of alcohol, or if you want to
concentrate diluted tincture you can basify it before boiling off the bulk of
the solvent.
It's all explained in Osmium: "Re: 7% tincture blues" (Stimulants)
Also, H2O2 reacts rather slow with iodides. Don't add too much, and don't add
it too fast. Excess H2O2 will oxidise the I2 into colourless, water-soluble
MIOx. So leave that reaction alone until all the I2 has
precipitated and the supernatant liquid is tea coloured or near colourless.
Might take a while, just leave it alone for a few hours or even overnight. If
you accidentially added too much H2O2 you can reverse that by adding more
tincture.
If you can get your hands on iodate (or even periodate), get it! This is by
far the best oxidiser for I2 production, the yields are almost quantitative.
I'm not
fat just horizontally disproportionate.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
07-12-02 18:22
|
|
|
|
Drying
& Storage
(Rated as: misinforming)
|
Bookmark
Reply
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Osmium
(Stoni's sexual toy)
07-12-02 18:58
No 331753
|
|
|
|
I2
will not be affected by light.
|
Bookmark
Reply
|
|
|
I2 will not be affected by light. It stores just fine in glass containers, it
even comes in glass containers.
I'm not
fat just horizontally disproportionate.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
(Couch HOG/Conversation DOMINATOR)
07-13-02 14:39
No 332042
|
|
|
|
I2
& light & stotage
|
Bookmark
Reply
|
|
|
"Iodine crystals have a very long shelf life if kept dry and in the
dark."
(Source: http://www.glaciermedicaled.com/Earthquake_html/Water/Water3.html
)
"I2 is light sensitive and will degrade. When completely dry store in
light resistant container.."
(Source: http://www.angelfire.com/mi3/chemhead/iodineconvert.html
)
"Bottle must be tightly capped when not in use to prevent vaporization
of iodine crystals."
(Source: http://www.polarequipment.com/page2.html )
The
early bird may get the worm, but the second mouse gets the cheese.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
lugh
(Moderator)
07-13-02 14:49
No 332047
|
|
|
|
Reagent
Grade Iodine
|
Bookmark
Reply
|
|
|
Reagent Grade Iodine is packaged and marketed in amber glass containers 
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
(Couch HOG/Conversation DOMINATOR)
07-13-02 14:55
No 332049
|
|
|
|
!!
|
Bookmark
Reply
|
|
|
Gee, I wonder why - Os!
The
early bird may get the worm, but the second mouse gets the cheese.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
hypo
(Official Hive Approximator)
07-13-02 15:30
No 332056
|
|
|
|
check
your sources!
|
Bookmark
Reply
|
|
|
methadist: while i don't know for sure if iodine is light senstive or not
(what should happen to it??), your sources prove absolutely nothing.
> "Iodine crystals have a very long shelf life if kept dry and in the
dark."
blah blah standard sentence. does it say that light is bad? no.
> http://www.angelfire.com/mi3/chemhead/iodineconvert.html
a tweeker reciepe. irrelevant.
> "Bottle must be tightly capped when not in use to prevent
vaporization of iodine crystals."
totally unrelated. vaporization has nothing to do with deterioration.
vaporization means that the iodine tranforms into a gas -
just because light goes in doesn't mean that iodine can
come out.
so either you come up with relevant refs (what _does_ happen to the
iodine under light influence), or...
lugh: maybe iodine is sold in dark bottles for esthetical reasons?
i'd get nervous, when the whole bottle is turning red... 
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
lugh
(Moderator)
07-14-02 01:31
No 332211
|
|
|
|
Vaporization
|
Bookmark
Reply
|
|
|
Iodine slowly sublimes at room temperature, so the main caution is to keep it
sealed, none of SWIL's books says anything about light sensitivity That
doesn't prove anything, except it's obvious that stating:
Never
store in glass or opaque containers
is trolling in the Stimulants forum, a very bad idea 
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Osmium
(Stoni's sexual toy)
07-15-02 17:04
No 332830
|
|
|
|
>
lugh: maybe iodine is sold in dark bottles ...
|
Bookmark
Reply
|
|
|
> lugh: maybe iodine is sold in dark bottles for esthetical reasons?
> i'd get nervous, when the whole bottle is turning red...
Every glass container I've received so far from a chemical supplier like
Merck, Fluka, Aldrich etc. was amber. Doesn't mean anything at all. If the
packaging is glass then it will be amber. They put everything into an amber
bottle by default.
I'm not
fat just horizontally disproportionate.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
07-15-02 21:32
No 332928
|
|
|
|
I2 +
light = 2I
|
Bookmark
Reply
|
|
|
Light liberates free iodine from crystals. This does not recombine
immediately. After long periods of time this can build up and recombine
explosively. Hence the dark bottles.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
07-15-02 22:30
No 332941
|
|
|
|
That
is utter bullshit.
|
Bookmark
Reply
|
|
|
That is utter bullshit.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
budstead
(Hive Bee)
07-16-02 04:37
No 333076
|
|
|
|
Hasn't
anyone read Vogal, Practical Chem circa ...
|
Bookmark
Reply
|
|
|
Hasn't anyone read Vogal, Practical Chem circa 1956. In one reaction
sodium iodide is formed. He writes a brief but thought provoking one
liner for the reclamation of the I2. SWIB will not give details, read
the book. But, he does indicate that sodium iodide + sodium dichromate+
Sulfuric acid + H2O makes for an interesting time. Give it a try.
One might want to try Potassium Dichromate + Potassium Idodide +
sulfuric acid + H2O. Please don't respond with any theoretical
bullshit, until you do the work. Than smile, fast clean robust.
Sorry this has nothing to do with tincture. Oh all the stuff is easy
and none alarming to get.
"That
Boys Not Right"
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
former_chemist
(Hive Bee)
07-16-02 06:53
No 333129
|
|
|
|
May
be bullshit
|
Bookmark
Reply
|
|
|
It may be bullshit. Never seen it happen. That is from one of
those NFPA (national fire protection agency) chemical hazard guides.
Light definitely causes disassociation but I can't see it doing more than
popping a cork. Chloroacetone supposedly does something similar, that I
have seen, hence using water or calcium carbonate as a stabilizer.
Edit:Found a number of references
that iodine is a stability hazard and heat and light are to be avoided.
No other description other than "free iodine is liberated".
Also found a reference to an iodine laser exploding. They use iodine in
lasers?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
budstead
(Hive Bee)
07-19-02 15:02
No 334568
|
|
|
|
SWIB
|
Bookmark
Reply
|
|
|
has seen it work, and work well.
"That
Boys Not Right"
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
07-24-02 20:02
No 336603
|
|
|
|
But...?
Doesn't iodate and iodide form I2?
|
Bookmark
Reply
|
|
|
Compound Formation between Sodium Iodate and Sodium Iodide
JACS 56, 295 (1934)
The complex formed between sodium iodate and sodium iodide has been shown not
to be a solid solution but to consist, in the temperature range between 20-55C,
of three double salts: 2NaIO3.3NaI.20H2O, 2NaIO3.3NaI.15H2O
and 2NaIO3.3NaI.10H2O.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
rocketfuel
(Stranger)
08-01-02 20:34
No 339856
|
|
|
|
Formula
i have been using and my return is 38 gr ...
|
Bookmark
Reply
|
|
|
Formula i have been using and my return is 38 gr and it has been firing up
very well,no problem buying for my horse with two left hoofs
1 pint 7% tincture iodine
3 pints of hydrogen peroxide
2 oz of HCl
1/2 cup of d-H20
in order put in 3 liter soda bottle,shake the wholly
wait 25 min,flakes are on the buttom ,rinse till the color
stays the same .it must be taken with care ,other wise it be yellow
everywhere
i love my glass .don`t need no grass ,make my fuel and have some class
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Osmium
(Stoni's sexual toy)
08-02-02 11:06
No 340167
|
|
|
|
>
But...? Doesn't iodate and iodide form I2?
|
Bookmark
Reply
|
|
|
> But...? Doesn't iodate and iodide form I2?
Yes, as soon as you acidify it.
I'm not
fat just horizontally disproportionate.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
(Couch HOG/Conversation DOMINATOR)
08-18-02 09:20
No 346382
|
|
|
|
Hate
to beat a dead horse, but...
|
Bookmark
Reply
|
|
|
From a "safety sheet" for I1 & I2 by JT Baker Chemicals
Inc.:
"Store separately from reactive or combustible materials, and out of
direct sunlight"\
Source: http://anon.user.anonymizer.com/http://www.jtbaker.com/msds/i2680.htm
The
early bird may get the worm, but the second mouse gets the cheese.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
chemicalwaste82
(Stranger)
08-27-02 04:41
No 349480
|
|
|
|
OK
|
Bookmark
Reply
|
|
|
Hardly a chemist here ,
swim just uses 7 % ratio 1 liter bottle of iodine
uses 2 bottles of peroxide 3 % lets sit in a gug overnite
pours through coffe filter puts on a small fan back drys
it yeilds 40 grams ussaly
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
(Amerikanskiy govn'ook)
10-09-02 20:18
No 366555
|
|
|
|
!!!
|
Bookmark
Reply
|
|
|
"Store out of light."
http://www.rhodium.ws/chemistry/iodine.tincture.html
The
early bird may get the worm, but the second mouse gets the cheese.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Osmium
(Stoni's sexual toy)
10-09-02 23:45
No 366611
|
|
|
|
You
can store it in bright sunlight for a hundred ...
|
Bookmark
Reply
|
|
|
You can store it in bright sunlight for a hundred years (as long as it is in
an airtight bottle), and the I2 will not deteoriate. It is an element, and
when there's nothing else around to react with its only chance of changing
into something else is radioactive decay.
I'm not
fat just horizontally disproportionate.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
(Amerikanskiy govn'ook)
10-10-02 00:46
No 366629
|
|
|
|
Shed
some light on the subject
|
Bookmark
Reply
|
|
|
Okay, but why does this prep as well as other internet references that I
cited say to "avoid light?
The
early bird may get the worm, but the second mouse gets the cheese.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
10-10-02 00:54
No 366633
|
|
|
|
It
is a standard phrase for storage of ...
|
Bookmark
Reply
|
|
|
It is a standard phrase for storage of everything, just like "in case of
skin contact, flush with large amounts of water".
Alcohol,
an unconsciousness-expanding drug
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
PoohBearium
(Bear With Me)
10-10-02 03:37
No 366692
|
|
|
|
Such
as...
|
Bookmark
Reply
|
|
|
...Rhodium: "Re: Electrochemical oxidations vs the
World" (Chemistry Discourse).
PB
I AM
a dog, but im not humping your leg, so quit kicking me!
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
methadist
(Amerikanskiy govn'ook)
10-11-02 21:36
No 367394
|
|
|
|
Light
Sensitivity (again)
|
Bookmark
Reply
|
|
|
RE: You
can store it in bright sunlight for a hundred years (as long as it is in an
airtight bottle), and the I2 will not deteoriate. It is an element
I wasn't referring to the composition - just the physical state. SWIM
remembers a batch that was left in the light and it began to liquify. But
this may have been due to unstable, poorly formed crystals.
So i'm doing a sunlight experiment with pre-fab crystals!
The
early bird may get the worm, but the second mouse gets the cheese.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Rhodium
(Chief Bee)
10-11-02 21:38
No 367395
|
|
|
|
The
melting point of Iodine is 113°C, so if it ...
|
Bookmark
Reply
|
|
|
The melting point of Iodine is 113°C, so if it was liquifying, it contained
something else.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
wr3cked
(Stranger)
10-29-02 03:29
No 373864
|
|
|
|
just
curious...
|
Bookmark
Reply
|
|
|
I have a bunch of lab grade hydrochloric acid... what would be the ammount
I'd use? 2 fluid ounces? For some reason it just seems wrong to me.
I admit to being generally green when it comes to chemistry, so if this is
foolish, let me know why.
I'd just rather know exactly what I'm dreaming before I even attempt to go to
sleep.
wr3cked
Life through
crystal eyes.
|
|
|
|
|
|
