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rstar
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Great Forum. Well this is my first post. 
I tried to make Na2CuCl4 by adding NaCl to CuCl2 solution, and the solution went from bluish to green. But I got problems, to get that stuff out of
the solution. 
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Chemistry Alchemist
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what is Na2CuCl4 used for? well are there any byproducts from the reaction? if not, then cant you just evaporate the solution?
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rstar
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Na<sub>2</sub>CuCl<sub>4</sub> = Sodium Tetrachlorocuprate(II)
Honestly I don't know any of its uses and I don't think that the reaction has any byproducts.
2NaCl + CuCl<sub>2</sub> = Na<sub>2</sub>CuCl<sub>4</sub>
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- Jöns Jacob Berzelius
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497
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I don't think that reaction exists. Do you have a reference for it?
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If it does exist and does work, then you should be able to simply evaporate away the solution to form Sodium Tetrachlorocuprate(II)
I guess if its a nice looking salt then it doesnt matter if it hasnt got any uses, may make a colour effect in a flame... Yellow + Green/Blue 
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rstar
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A Wikipedia page on CuCl<sub>2</sub>,
<a href="http://en.wikipedia.org/wiki/Copper(II)_chloride#Properties_and_reactions"> Here </a>
It tells that CuCl<sub>2</sub> reacts with chloride sources to form CuCl<sub>3</sub><sup>-</sup> and
CuCl<sub>4</sub><sup>2-</sup> ions.
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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Chemistry Alchemist
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So in other words if would make copper 3 or 4 chlorides insteaspd of reacting to make Sodium Tetrachlorocuprate(II) ?
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497
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Yeah it might work. Every preparation I've seen uses concentrated HCl though. The color change you observed could be the result of a small fraction of
tetrachlorocuprate forming.
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rstar
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Maybe yes
[Edited on 27-9-2011 by rstar]
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rstar
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Here's what i got after evaporation, sorry for bad picture quality :
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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Chemistry Alchemist
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Yeah I was going to say, where would the Sodium go if the copper gained another chlorine, would the copper 3 and 4 chloride make a better flame co our
then copper 2 Chloride? Or doesn't the extra chlorine make any Difference?
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Is this ur suposibly Sodium Tetrachlorocuprate(II)?
Because that kinda looks exectly like my copper (II) chloride
The picture on the Left is no flash and the one on right is with the flash... Copper (II) Chloride in a concerntrated solution is one colour, and once
dilute it turns another colour (cant remember if its blue to green or green to blue)
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Chemistry Alchemist
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ok for some reason my pictures didnt attach :/ prob coz if shit internet
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Arthur Dent
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@ rstar: A nugget of the purest green: http://www.youtube.com/watch?v=TkZFuKHXa7w
 Robert
--- Art is making something out of nothing and selling it. - Frank Zappa ---
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rstar
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I also think like that's just a mixture of CuCl<sub>2</sub> and NaCl. The complex might have decomposed as I got all solvent evaporated.
Maybe the complex is only stable in solution form.
"A tidy laboratory means a lazy chemist "
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rstar
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@Arthur Dent
Thanx for the video link, that man has done the "Green" gold, it might be eco friendly
"A tidy laboratory means a lazy chemist "
- Jöns Jacob Berzelius
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rstar
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They are not Copper 3 or 4 chlorides
they are:
CuCl<sub>3</sub><sup>-</sup> = Trichlorocuprate(II) ion
CuCl<sub>4</sub><sup>2-</sup> = Tetrachlorocuprate(II) ion
"A tidy laboratory means a lazy chemist "
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LanthanumK
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When copper(II) is crystallized out of an acidic solution, it forms green crystals, such as my CuCl2. This is probably due to the presence of
moisture, which allows CuCl4(2-) ions to be in there. When dried further, it turns bluer as the rest of the HCl is driven off, leaving aqua ions
behind.
hibernating...
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Mixell
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NaCl and CuCl2 have different solubility, and I don't know about the solubility of NaCl in concentrated HCl, what you got is most certainly a mixture
of NaCl and CuCl2, may be a small amount of CuCl3 -1/CuCl4/ 2- in there...
Those complexes are usually made with cesium/rubidium, mostly cesium. CsCl in soluble in concentrated HCl, whereas the complex salt is not.
Here is a detailed preparation of those salts and a bit of information about them: http://woelen.homescience.net/science/chem/exps/CsCuCl3/inde...
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Precipitation of Copper Phosphate
Sorry to change the subject but i made Copper Phosphate by reacting Phosphoric Acid with Copper Oxide, i now hve a deep Blue solution of copper
phosphate, ive wanted the solution to evaporate to form the precipitate but for some reason it isnt evaporating... how can i precipitate it out? can i
add more water to it? Copper Phosphate is insoluble in water but soluble in phosphoric acid... could this work?
Another method is reacting the solution with Sodium Carbonate, this will react with the acid to neutralize it and and precipitate the Copper Phosphate
but because the Copper Phosphate is in solution, would the Sodium Carbonate also react with the Copper Phosphate to Form Copper Carbonate and Sodium
Phosphate?
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bbartlog
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If you have a deep blue solution I would assume you have excess phosphoric acid, since copper phosphate is insoluble. What quantities of reagents did
you use? Ideally it seems like you should add more CuO until all the phosphate is thrown down, but dilution might also work. It should be easy enough
to draw off a few ml of your solution and dilute it with 20x its volume in water to see what happens.
As for the sodium carbonate idea, yes, I suspect you end up with copper carbonate and sodium phosphate.
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i just added CuO untill it hardly fizzed, so do you suggest keep adding the CuO untill no more dissolves? yeah ill try dilute a small proportion of it
and see what happens
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