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Toluene
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My iron salts collection
Hi everyone!, in this photo I show you my Iron salts collection
I know that it's still small, but I'm planning to do some Iron nitrate, mohr's salt and iron acetate, I'd like to do also citrate and a ferrate salt
such as sodium ferrate, but I don't know if it is going to be stable in solid form, and for the case of citrate I don't know nothing about its
production
Any recommendations for making the family bigger? 
The last one, is this pink- brownish compound, synthethised this evening wich is Iron III aspirinate
Cheers!
[Edited on 12-1-2014 by Toluene]
[Edited on 13-1-2014 by ScienceSquirrel]
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alexleyenda
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Looks great Challenge (I guess) suggestion : Iron Bromide (make it yourself
:p )
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Toluene
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Thank you alexleyenda! unfortunately I don't have acces to any bromide or any
source of bromine in order to prepare hydrobromic acid 
btw, al the salts have been prepared by me from iron metal (steel wool)
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Random
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Iron citrate might be easily attacked by moulds as many other citrate salts
Iron ammonium citrate is photosensitive and you can make some blueprints or whatever those photographic papers are called
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Toluene
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Thanks Radom, is then any way to synthesis the citrate or the iron ammonium citrate?
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alexleyenda
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Quote: Originally posted by Toluene  | Thank you alexleyenda! unfortunately I don't have acces to any bromide or any
source of bromine in order to prepare hydrobromic acid
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That was what I thought, that's why it's a challenge :p by the way, a source is not so hard to find, it took me 10 seconds on the website of a local
pool store http://www.clubpiscine.ca/417-product-spas-hot-tubs-maintena...
[Edited on 12-1-2014 by alexleyenda]
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cyanureeves
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Toluene have you ever heard of oil of iron?it is not a salt but it is a sweet smelling oily stuff made with iron sulfate or pyrite,(nitric acid?)and
acetone i believe.i used to could google it and it would come up but lately i cant get nothing.potassiumferrocyanide would be good salt for you and
the prettiest ferrycyanide.iron sulfate and aspirinate are so gentle looking it's almost therapeutic and to think these salts come from cold mean
rugged steel.mean?so i guess iron salicylate is the word for it?
[Edited on 1-12-2014 by cyanureeves]
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Random
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Mix iron hydroxide with citric acid and then add ammonia. Then again add citric acid until no precipitate is seen with ammonia.
There are several forms depending on reagent ratios. Remember it can catch mould easily, maybe there is something that can be added to prevent it?
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Zephyr
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Nice collection, some other possible additions would be Iron thiocyanate and Iron oxalate.
[Edited on 12-1-2014 by Pinkhippo11]
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Brain&Force
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Try ferric sulfate, ferrous chloride, ferrous oxide, magnetite, or ferrous iodide. Ferric alums would be interesting. Some nice, unusual ones could
include iron chromates, molybdates, tungstates, tantalates, niobates, and vanadates.
And what about something like ferrous or ferric ferrate? That would be really interesting.
At the end of the day, simulating atoms doesn't beat working with the real things...
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blogfast25
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Suggestion: ferric alum. Several preparations have been described on this forum.
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Toluene
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Thank you all for your advices! I will update this thread when I prepare more salts! Thank you!!
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Random
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You can also try to make ferrofluid.
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blargish
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Ferrous oxalate would be an interesting one as its thermal decomposition leaves pyrophoric iron particles
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DraconicAcid
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Potassium iron(III) oxalate forms nice green crystals.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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woelen
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This is a nice initiative and I like to see this kind of collections. I, however, have one remark about the storage of the compounds. You should not
use corked bottles, but bottles with a decent screw cap, which is not made of metal. E.g. FeCl3.6H2O and Fe(NO3)3.9H2O are quite corrosive and very
hygroscopic and these certainly interact with the cork in undesirable ways. FeSO4.7H2O is very prone to aerial oxidation and I'm quite sure that after
a few years of storage your ferrous sulfate is not looking nice mintgreen, but dirty green with brown spots in it.
Cork simply is not a suitable way of stoppering chemicals. It was used in the past, due to lack of better materials, but nowadays you should not use
it anymore for anything which is more permanent than for a few days.
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blogfast25
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http://www.sciencemadness.org/talk/viewthread.php?tid=20688
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Toluene
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Hi everyone! This evening I'm going to synthesis iron ammonium citrate, I will bring up with the results!
Thanks for your advice woelen, but the stop-corked vials are more classic and more elegant  , nah seriously, I don't have the acces to other vials by the moment, maybe in a few weeks I can buy, so I'll transfer them 
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Toluene
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By the way, a friend of mine who's a chemist helped me with the structure of the iron aspirinate
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woelen
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It is also interesting to make transient iron species. You cannot store them, but their formation and subsequent destruction is interesting to watch.
One nice example is addition of an iron(III) salt to a solution of sodium thiosulfate. This gives a beautiful purple solution, due to formation of a
thiocyanato complex of iron(III). This complex, however, is unstable, an internal redox reaction occurs, with the iron going to oxidation state +2 and
the thiosulfate being oxidized to tetrathionate.
A nice crystalline compound is potassium trisoxalatoferrate(III). You can make this by dissolving an iron(III) salt in a solution of oxalic acid and
potassium carbonate (or hydroxide). This complex forms nice green crystals, more like grass and not like the pale green iron(II) sulfate. K3Fe(C2O4)3
is sparingly soluble in cold water and can easily be recrystallized. You could also try to make the ammonium salt of this, which also can be
crystallized easily.
EDIT: I now see that DraconicAcid mentioned this chemical already before I did.
[Edited on 13-1-14 by woelen]
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Toluene
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Hi! I tried to prepare this evening ammonium ferric citrate, I disolved 10g of Fe(OH)3 in 50 mL of saturated solution of citric acid, then I added 50
mL of household ammonia, nothing seemed to precipitate, a brown solution is all i got, I didn't want to boil of the water, because I thought that an
excess of temperature may yield Fe2O3, so I have the solution evaporating and I don't know If I've done it right
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Random
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Color and properties of this product are highly dependant on the ratios of reactants. Also there might be some purification needed as there might also
be ammonium citrate etc.. It's not so simple but you may try some experiments with it, especially you have ferrocyanide. You can search for blueprint
experiments or also research ratios of reactants.
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Zyklon-A
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How about, Iron oxide (FeO), Iron persulphide FeS2, Iron nitrate hexahydrate: Fe(NO3)2.6H2O, Iron iodide
tetrahydrate: FeI2.4H2O, Diiron trisulphate nonahydrate: Fe2(SO4)3.9H2O.
[Edited on 14-1-2014 by Zyklonb]
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Poppy
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Go for Iron benzoate, iron ammonium phosphate (which is said to be blue but the green variant most common)
Yeah its hard to remove the last 2 water molecules out of the citrate which makes it very fluffy for bateria to eat through.
| Quote: Originally posted by Random |
Iron ammonium citrate is photosensitive and you can make some blueprints or whatever those photographic papers are called |
Genius! genius!
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a_bab
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Besides the interesting pyrophoric-iron experiment iron oxalate can be used to make holograms (preferably with blue laser).
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