Draeger
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Getting HCl to react with copper metal?
I have a bit of HCl sitting on top of what supposedly looked like copper oxide. After I added HCl, though, I saw that there was now a red solid, which
was copper, which was the most part of what was supposedly copper oxide. Now I have to get the HCl to react with the copper.
I was thinking about boiling off water from my very dilute 3% H2O2, but I don't have much of it, and it would also be really dangerous. So I was
hoping that maybe a few drops with most of their water boiled off would be enough to get the reaction going, but I am really not sure how rigorous the
decomposition would be if I overshot the goal. Or maybe there is an alternative to H2O2?
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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Bedlasky
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I think that 3% H2O2 should be fine. Mix solutions and heat it.
You can use any source of nitrate instead of H2O2.
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reactofurnace
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Is your goal to make Copper (II) chloride? If so the 3% H2O2 should work just fine. You could also bubble air into the mixture, however, this might be
slow. In addition, I read on Wikipedia that the reaction of copper oxide and ammonium chloride is feasible (at temps of about 300deg celsius)
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Draeger
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Quote: Originally posted by Bedlasky  | I think that 3% H2O2 should be fine. Mix solutions and heat it.
You can use any source of nitrate instead of H2O2. |
Could I safely boil off the solution that I have now? It still contains some H2O2.
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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Bedlasky
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Yes, but do it outside, because of chlorine formation.
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Draeger
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Is there some way I could prevent chlorine formation? I can't do it outside, and there is no well-ventilated place in my home, either.
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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Texium
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Thread Moved
21-4-2020 at 14:05 |
Herr Haber
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In front of a window, remove anything metallic from the immediate surroundings, if possible blow a fan.
But I dont think you'll be producing a worrying amount of chlorine anyway. Just dont stay around in the room if you cant do it outside.
The spirit of adventure was upon me. Having nitric acid and copper, I had only to learn what the words 'act upon' meant. - Ira Remsen
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lordcookies24
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I did this 2 years ago with 3% H₂O₂ to get CuCl₂ and it catalyzed it very well. Be sure to heat the solution well and if you have magnetic
stirrer use it. Also I did this outside and it is a good thing I did because I might have heated it up a bit too much cause when I came outside after
an hour my porch was well decorated with CuCl₂ crystals splattered all over .
[Edited on 25-4-2020 by lordcookies24]
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