White Yeti
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Synthesis of sodium thiocyanate.
Note: I know I can just buy the stuff, but I want to try to synthesise it myself, just for the hell of it.
I will attempt to synthesise sodium thiocyanate very soon, as soon as the urea I extracted from fertiliser comes out of solution.
In the meantime, I wanted to make sure the way I'm going about this synthesis is correct.
I worked out the heat of reaction involving the conversion of sodium carbonate and urea to sodium cyanate, water, ammonia and carbon dioxide (
endothermic +210KJ/mol).
The reduction of cyanate to cyanide with carbon powder was also endothermic (about 420KJ/mol, a little less if carbon is converted to dioxide instead
of monoxide).
But the conversion of cyanide to thiocyanate is exothermic (-680KJ/mol), so much so, that the heat released in this step would cancel out the heat
requirement of the other two initial steps, increasing the chances of success for this reaction.
But I'm afraid that dumping all these reactants into one big reaction vessel (made of steel, this may be a problem) would suffer from many side
reactions that would severely lower yield. I fear that the sulfur may boil off, as its boiling point is quite low.
I have limited equipment, a charcoal furnace, and it's much more convenient for me to perform this synthesis in one step rather than 3. But, I'm not
going to do it if the yields will be extremely low.
Which is better, mixing everything in one big step, or performing every step separately?
"Ja, Kalzium, das ist alles!" -Otto Loewi
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kmno4
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Your methode will not work.
"conversion of cyanide to thiocyanate is exothermic (-680KJ/mol)"
- very improbable and surely wrong value. How did you calculate it ?
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plante1999
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If you do every step separately, it will give better yield , sulfur adition to cyanide is endothermic.
I never asked for this.
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kmno4
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No, it is not.
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plante1999
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Mayby I made a mistake but in solution, from wath I remenber, the cyanide sol. need to be heated to disolve the sulphur.
[Edited on 16-1-2012 by plante1999]
I never asked for this.
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plante1999
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Maybe sulphur reduction of cyanates is possible? If C can reduce cyante I suppose S8 could to....
More research is needed here.
I never asked for this.
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White Yeti
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Quote: Originally posted by plante1999  | Maybe sulphur reduction of cyanates is possible? If C can reduce cyante I suppose S8 could to....
More research is needed here. |
That's not a bad point, but I'm afraid that the sulfur could potentially boil off before reducing the cyanate. This is definitely not an issue with
carbon, which is both more accessible and better at removing oxygen than sulfur.
I was thinking about reducing cyanate with carbon and having sulfur in the same vessel to react with the subsequent cyanide salt. I'm wondering if
this method would also generate carbonyl sulfide, as carbon is oxidised to CO and then to COS as sulfur is in close proximity.
"Ja, Kalzium, das ist alles!" -Otto Loewi
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blogfast25
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WY:
I'd definitely research your subject a helluvalot more, if I were you!
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Random
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Anyone has some new information on this subject? Would cyanate react with sulphur while heating it to form thiocyanate?
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AJKOER
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Per Atomistry.com (see https://www.google.com/search?newwindow=1&site=&sour... ) to quote:
"The salts of thiocyanic acid are generally obtained by the direct action of sulphur or a polysulphide on the cyanide, by the action of hydrogen
cyanide or cyanogen on a polysulphide,
(NH4)2S2 + HCN = NH4CNS + NH4HS,
Na2S2 + (CN)2 = 2NaCNS,
or by the decomposition of a complex cyanide by fusion with an alkali carbonate and sulphur.
The thiocyanates are generally soluble in water, the exceptions being those of lead, silver, mercury and copper. Most of them dissolve also in
alcohol and ether. Aqueous solutions of the alkali thiocyanates undergo atmospheric oxidation under the influence of sunlight; with solutions of
medium concentration this change takes place rapidly, with separation of a yellow, amorphous precipitate consisting of pseudo-cyanogen sulphide,
(CNS)3. The concentration of thiocyanate most favourable to the separation of this sulphide is about 50 per cent, in summer and 10 per cent, in
winter. In addition to this substance the products of the photochemical oxidation of potassium thiocyanate include hydrocyanic acid, sulphate, carbon
dioxide, ammonia and ammonium salts:
12KCNS + 12O2 + 6H2O = 6K2SO4 + 3HCN + 3CO2 + 3NH3 + 2(CNS)3.
An unstable intermediate peroxygenated compound is also always formed. This gives a blue coloration to fresh guaiacum tincture and is possibly
analogous to Caro's acid.
Any pink colour that may develop in solutions of alkali thiocyanates on exposure to light is due to oxidation of traces of ferrous salts usually
present by dissolved oxygen."
I would add CuCl2 or CuCO3 to form the insoluble Copper salt.
--------------------------------------------------
Another possible path (probably need more info on any catalyst, reaction temperatures,..., which was discussed previously on Sciencemadness no less,
see http://www.sciencemadness.org/talk/viewthread.php?tid=17892#... ) per Wkipedia (http://en.wikipedia.org/wiki/Ammonium_thiocyanate ):
"Ammonium thiocyanate is made in the United States by the reaction of carbon disulfide with aqueous ammonia. Ammonium dithiocarbamate is formed as an
intermediate in this reaction, which upon heating, decomposes to ammonium thiocyanate and hydrogen sulfide:
CS2 + 2 NH3(aq) → NH2C(=S)SNH4 → NH4SCN + H2S"
Interestingly, the patent cited in the prior SM thread
(ww.google.com/patents?id=ICltAAAAEBAJ&pg=PA2&dq=manufacture+carbon+disulfide&hl=en&ei=VQStTse0McWCtgejwLHYDg&sa=X&oi=book_res
ult&ct=result&resnum=7&ved=0CEAQ6AEwBjgK#v=onepage&q=manufacture%20carbon%20disulfide&f=false ) notes on the 1st page 2nd
paragraph, the need for diluents for the reaction to occur, and the use of water, alcohol,... may actually result in Ammonium thiocyanate (our goal).
If created, I would add CuCO3 to form a precipitate, or just add NaHCO3 and heat to isolate the NaCNS.
--------------------------------------------------------------
On how to prepare CS2, per Atomistry.com (http://sulphur.atomistry.com/carbon_disulphide.html ) to quote:
"Carbon disulphide is prepared by passing sulphur vapour over red hot charcoal. The preparation may be carried out on a small scale by heating pieces
of charcoal in a combustion tube placed in a furnace slightly tilted, a Liebig potash bulb, immersed in ice, being attached to the lower end of the
tube, and small pieces of sulphur introduced into the upper end of the tube which is then closed with a cork. Sulphur vapour passes over the red-hot
charcoal and impure carbon disulphide containing sulphur in solution is gradually formed and collects in the cooled receiver. The reversible reaction
C + 2S ⇔ CS2 "
-----------------------------------------------
I would find the formation of Ammonium thiocyanate interesting as per, for example, "Synthesis of aryl thiocyanates using Al2O3/MeSO3 H (AMA) as a
novel heterogeneous system " link: http://www.ingentaconnect.com/content/stl/jcr/2008/00002008/... to quote:
"Indoles and various aromatic and heteroaromatic compounds undergo smooth thiocyanation with ammonium thiocyanate in the presence of a mixture of
Al2O3/MeSO3H (AMA) under mild conditions without use of any organic solvents to afford the corresponding aryl thiocyanates in excellent yields and
with high selectivity."
and then, using chlorobenzene, as an example of an aryl (C6H5) chloro derivative, a possible reduction of C6H5SCN to the cyanide as cited in this
reference "Electrochemical Reduction of Aryl thiocyanates: A Unique Autocatalytic Process and Evidence for a Concerted-Stepwise Mechanism Transition",
link: http://www.electrochem.org/dl/ma/203/pdfs/2563.pdf where the author lists the reactions:
ArSCN + 2e ---> ArS- + ArSCN-
ArS- + ArSCN ---> ArSSAr + CN-
ArSSAr + 2e ---> 2 ArS-
although the absence of more specifics is disappointing.
------------------------------------------------------------------------
Here is a reference on the preparation of methane sulfonic acid (or, MeSO3H per US patent 6207025) by irradiating a mixture comprising acetic acid,
sulfur dioxide and oxygen with light, link: http://www.google.com/patents/US6207025 .
[Edited on 19-1-2014 by AJKOER]
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Fantasma4500
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polysuphides..
if sulfur doesnt work out you could try polysuphides as stated above
of what i recall about golden powder, an interesting mixture, supposedly polysulphides are formed aswell as nitrogen sulfides
3:2:1 KNO3 K2CO3 S
if the 2 parts K2CO3 and 1 part S is mixed and heated beforehand it should form polysulphides which will when mixed with the 3 parts KNO3 all finely
powdered burn violently, as the polysulphides acts as a fuel, reaching 8 times the burn speed of blackpowder
~~you can make polysulphides by melting K2CO3 with S~~
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Random
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But I asked for cyanate not cyanide
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Fulmen
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Random: Did you solve this? I too am looking for a non-cyanide route to thiocyanates, preferably from sodium cyanate.
We're not banging rocks together here. We know how to put a man back together.
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XeonTheMGPony
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https://www.bitchute.com/video/0dMUS0GfPkgG/
Older thread but been researching this as of late.
May be helpful.
Sodium thiosulfate by sodium bisulfite route.
(And this kids is why you shouldn't do any thing when tired! wrong substance entirely far as thread topic goes!)
[Edited on 22-9-2019 by XeonTheMGPony]
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Bedlasky
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If I know thiocyanates are produce in laboratory by heating potassium ferrocyanide with sulfur.
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rockyit98
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better yet you could heat Prussian blue with thiosulfate or sulfur .
https://en.wikipedia.org/wiki/Prussian_blue
https://en.wikipedia.org/wiki/Thiocyanate
if you want sodium salt you can melt the mixture with NaOH.
[Edited on 22-9-2019 by rockyit98]
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rockyit98
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https://en.wikipedia.org/wiki/Thiourea
https://en.wikipedia.org/wiki/Ammonium_thiocyanate
[Edited on 22-9-2019 by rockyit98]
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XeonTheMGPony
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https://www.ebay.ca/itm/Natriumthiocyanat-SODIUM-THIOCYANATE...
found this source, yet to order so can't say of quality, but I can say last several chemical orders from said country been exceptional quality
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BAV Chem
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Thiocyanate from NaCN and sulfur
I'm currently trying to make thiocyanate by refluxing a solution of NaCN over sulfur. My cyanide is far from pure as I made it by heating a mix of
Na2CO3, urea and carbon.
At the start the reaction worked well but then after I added the second half of my sulfur it started forming polysulfides in solution and stopped
producing more thiocyanate. To make a long story short I then did some research and found that I have an ammonium contamination in there which will do
anything to inhibit thiocyanate formation.
Where's that ammonia from? Some urea pyrolysis product maybe?
Any suggestions how to mitigate that apart from purifying the cyanide (which I want to avoid)?
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Bedlasky
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I doubt that you have ammonia in your solution. Your impure NaCN contain some sodium carbonate. Sodium carbonate will react with excess of sulfur to
form polysulfide.
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Boffis
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Hi BAV Chem, I used to prepare my own thiocyanates until I discovered I could buy them so cheaply and easily. It is best to isolate the cyanide as a
ferrocyanide salt first and then fuse this with sulphur. The easiest way to isolate the cyanide ions is to add a mixture of ferric and ferrous salts
to the weakly alkaline mixture of and filter off the crude prussian blue, suspend it in clean water and then treat this with a strong (10-12% solution
sodium or potassium hydroxide solution) until the suspended solid has turned a plain-chocolate-brown colour and filter. It is best to let the
suspension settle overnight and decant as much clear liquid first as the ppt is a bitch to filter although kieselguhr addition helps a lot. The pale
yellow solution is the simply evaporated down until a small sample crystallises on cooling. By this point the solution will have turned cloudy and
brown and require treatment with charcoal and kieselguhr mixture and filtering hot to obtain a clear solution. The crystals of ferrocyanide are
usually very pure. The conversion of ferrocyanide into thiocyanate or back into purer cyanide is widely reported.
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BAV Chem
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Hello Boffis, I know I can actually order some thiocyanate on amazon rather easily but I'm still trying to make some for fun. Also who knows maybe in
a while even thiocyanate will be hard to come by. Very nice ferrocyanide preparation btw 
Also Bedlasky, I do actually know for a fact that there's an ammonia contamination as it fumes when I bring some HCl close. You're right about there
being carbonate as a major impurity but weirdly enough there's still cyanide in solution which should react with the polysulfides but it doesn't...
even after boiling out any ammonia it somehow doesn't react fully. Perhaps there's some thiocyanate <--> cyanide+sulfur equilibrium going on
there.
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