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Texium
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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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I think it disproportionated into manganese dioxide and permanganate as the solution became less basic.
At the end of the day, simulating atoms doesn't beat working with the real things...
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bismuthate
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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
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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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Amos
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Maybe see if it is repeatable? You might be headed towards a whole new class of colored solutions for me to collect
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gdflp
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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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Fantasma4500
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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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Brain&Force
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I wonder if manganese(II) permanganate is stable.
Happy 1001st post Antiswat.
At the end of the day, simulating atoms doesn't beat working with the real things...
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bismuthate
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Well no, I don't think it could be because Mn(II) is oxidized by permanganate.
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TheChemiKid
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What about Mn(IV) Permanganate?
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bismuthate
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I would think Mn(III) permanganate would be more likely.
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Texium
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So you mean something like Mn(MnO4)3?
Err... I think not.
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bismuthate
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Well yeah it would probably just make Mn2O3.
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Texium
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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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Fantasma4500
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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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prof_genius
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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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bismuthate
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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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j_sum1
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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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bismuthate
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It's most likely Mn+3, but I can't conclude anything beyond that.
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Eddygp
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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.
there may be bugs in gfind
[ˌɛdidʒiˈpiː] IPA pronunciation for my Username |
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Molecular Manipulations
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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.
-The manipulator
We are all here on earth to help others; what on earth the others are here for I don't know. -W. H. Auden
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kecskesajt
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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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quantumcorespacealchemyst
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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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Molecular Manipulations
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A chalcogenide? Could you be any more vague about the nature of this chemical?
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I am unsure if heating and or refluxing/boiling will cause an accelerated reaction/runaway reaction.
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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.
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Please advise me on the safest approach.
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Find the nearest toxic waist processing facility and throw away your entire <s>lab</s> reaction.
[Edited on 25-2-2015 by Molecular Manipulations]
-The manipulator
We are all here on earth to help others; what on earth the others are here for I don't know. -W. H. Auden
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quantumcorespacealchemyst
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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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