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Author: Subject: The "WTF did I just make?" thread
Texium (zts16)
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[*] posted on 31-8-2014 at 17:02
The "WTF did I just make?" thread


Thought I'd make a thread for when you are trying to do one thing, and then something totally unexpected happens instead. (Not sure if this phenomenon happens to everybody. It certainly happens to me a lot!)

To start it off, I was experimenting with various manganates. One that I made is what I think is calcium manganate (Hard to tell though, since there is almost no information about it out there. It isn't even in the CRC handbook). Anyway, I made it from solutions of K2MnO4 and CaCl2. It formed a purple-mauve precipitate, and the solution turned purple. The weird thing though was that after I vacuum filtered it, the purple solution turned red and turbid, and the CaMnO4 precipitate turned beige. I think what caused this was me not cleaning my büchner funnel well enough. (It smelled a little bit like chlorine still from MnO2+HCl)

I still have absolutely no idea what compounds were formed, but the red color is fascinating and totally unexpected!




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Brain&Force
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[*] posted on 31-8-2014 at 21:27


I think it disproportionated into manganese dioxide and permanganate as the solution became less basic.



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bismuthate
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[*] posted on 1-9-2014 at 04:51


I will be using this thread so much. :)
When i mixed solutions of Iron (III) chloride (with some ferrous in it possibly) and a small amount of sodium chromate I got a grey precipitate. What's this? could it be iron chromium oxide formed by ferrous ions?




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Texium (zts16)
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[*] posted on 1-9-2014 at 08:37


Quote: Originally posted by Brain&Force  
I think it disproportionated into manganese dioxide and permanganate as the solution became less basic.
That's what I thought at first too, but this stuff was really red! I'd seen the disproportionation happen a couple of times before and this looked completely different. I guess it will remain a mystery though. Since it was most likely caused by contaminants on the funnel, it would be quite difficult to repeat.



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[*] posted on 1-9-2014 at 08:43


Maybe see if it is repeatable? You might be headed towards a whole new class of colored solutions for me to collect:D



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[*] posted on 1-9-2014 at 12:01


As for WTF reactions, this one was quite a surprise for me http://www.sciencemadness.org/talk/viewthread.php?tid=32902
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[*] posted on 1-9-2014 at 13:17


i once tried making manganese sulfate, reacting MnO2 with ascorbic acid (which apparently is very useful??)
it turned brownish, and overall seemed to be Mn3O4
then i attempted to react this new weird substance with H2SO4 and zinc metal powder, turned reddish
at some point i estimated out of others guesses that what i may have formed might be Mn2(SO4)3
i recall that it doesnt want to react very well with carbonates or anything alike

just thought i found a very neat method of making manganese salts that can be used, but apparently i just have some reddish clusterfuck now of some sort

http://puu.sh/bhsvh.jpg
ill just leave out trying to put it up here as a picture as its 100x800 and will fill entire page
as seen it has a nice colour, and its alot more clear than i recall it was
could do some reactions if anyone are interested in it etc




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[*] posted on 1-9-2014 at 20:29


I wonder if manganese(II) permanganate is stable.

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[*] posted on 2-9-2014 at 03:23


Well no, I don't think it could be because Mn(II) is oxidized by permanganate.



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[*] posted on 2-9-2014 at 04:40


What about Mn(IV) Permanganate?
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[*] posted on 2-9-2014 at 08:54


I would think Mn(III) permanganate would be more likely.



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[*] posted on 2-9-2014 at 13:39


So you mean something like Mn(MnO4)3?
Err... I think not.




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[*] posted on 2-9-2014 at 13:55


Well yeah it would probably just make Mn2O3.



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[*] posted on 2-9-2014 at 15:02


I think that what I made was probably MnCl3. I saw a picture of Mn(III) solution on woelen's site, and it looked quite similar. Also, it has since separated into a brownish solid and a clear solution, quite similar looking to his second picture of Mn(III).



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[*] posted on 3-9-2014 at 09:12


why dont you ask to have this thread stickied somewhere?? i think either other chemists does too simple reactions or are too proud to confess that they are confused over what the hell they have witnessed taking place infront of their eyes, perhaps im just one of the chosen few to get confused over what may once in a while happen in chemical reactions..
sticky thread!! you have my vote




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[*] posted on 3-9-2014 at 09:35


I was making iodoform yesterday and I must have gotten the proportions wrong because the solution turned blue and released white fumes that I believe where HCl gas. Has this happened to anyone?
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[*] posted on 19-1-2015 at 11:25


I performed this experiment:
I dissolved 5g of sodium molybdate in around 75mL of 3% H2O2.
I then mixed it with 50mL of a solution of what should be 2.5% copper acetate.
It formed a brown precipitate which settles rather slowly.
I doubt this is copper peroxomolybdate, but I can't think of another explanation for it. Does anybody know what this could be?

[Edited on 19-1-2015 by bismuthate]




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[*] posted on 19-1-2015 at 22:02


Quote: Originally posted by zts16  
To start it off, I was experimenting with various manganates.
[snip]
The weird thing though was that after I vacuum filtered it, the purple solution turned red and turbid, and the CaMnO4 precipitate turned beige. I think what caused this was me not cleaning my büchner funnel well enough. (It smelled a little bit like chlorine still from MnO2+HCl)

I still have absolutely no idea what compounds were formed, but the red color is fascinating and totally unexpected!


On a similar note, I have always wondered about the red at the end of this demonstration. I have never been able to duplicate it. I read woelen's description on manganates fully (linked upthread by zts16. So much to learn.) He never mentions this red either.

[edit faulty link]

[Edited on 20-1-2015 by j_sum1]
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[*] posted on 20-1-2015 at 04:21


It's most likely Mn+3, but I can't conclude anything beyond that.



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[*] posted on 20-1-2015 at 12:04


While cleaning some cheap glassware with ethanol, I noticed some small black specks from some previous experiment that I have conducted. Curiously enough, the specks dissolved in the ethanol yielding a vivid purple colour. I have been working with ammonium phosphates, iodides, sodium hydroxide and hexane. Any ideas? I don't think that it is iodine.



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[*] posted on 20-1-2015 at 12:24


Why don't you think it's iodine? You had iodide present. Iodide can easily be oxidized to iodine. Where there any oxidizers?
Small amounts of iodine can make for a very bright purple color in ethanol.




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[*] posted on 13-2-2015 at 11:17


I tried to make 2-propyl nitrite with homemade KNO2 wich is made using KNO3 and lead metal.So I mixed 2-propanol with the nitrite, cooled down and added H2SO4 in small portions.At first it turned yellow than into a black-gooey.Smells like a car motor but 20 times more concentrated.Can somebody help?
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[*] posted on 25-2-2015 at 11:39
Hg, Hg sulfates (I, II), KNO3, H2SO4, K2S2O8


I have small unknown amount of Hg and Hg sulfates with 4.314gKNO3, 3.8ml 98% H2SO4, 5ml H2O and 6.531g Potassium persulfate (K2S2O8). It was combined at around room temperature and kept colder. No reaction yet.

I am unsure if heating and or refluxing/boiling will cause an accelerated reaction/runaway reaction.

Please advise me on the safest approach.

I have 0.998g of a calcogenide I want to add, and moniter it's reaction rate at around boiling. Before doing this, I am concerned with the nature of getting the reaction mix I have described, safely to the boiling point/reflux and get a good idea of it's own reactivity (thermodynamic behaviour?), prior to monitering another reagent addition.


thanks

[Edited on 25-2-2015 by quantumcorespacealchemyst]
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[*] posted on 25-2-2015 at 12:08


A chalcogenide? Could you be any more vague about the nature of this chemical?
Quote:

I am unsure if heating and or refluxing/boiling will cause an accelerated reaction/runaway reaction.

I'm unsure, of what reaction you want to happen. But I'm sure it won't be a "runaway". Everything here is as oxidized as it could be (except half of the mercury is in the 1st oxidation sate), I can't think of a single reaction that could happen at all.
Quote:

Please advise me on the safest approach.

Find the nearest toxic waist processing facility and throw away your entire <s>lab</s> reaction.


[Edited on 25-2-2015 by Molecular Manipulations]




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[*] posted on 25-2-2015 at 12:12


Do you think that an oxidizer {KNO3} is too unreactive with an O2 source {K2S2O8}? the reactants are mixed and cold. the calcogenide is 0.998g Tm2Te3.

I don't believe I understand the action of K2S2O8 well.


[Edited on 25-2-2015 by quantumcorespacealchemyst]
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