Camroc37
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How is this reaction possible?
So something I thought wasn't possible happened:
I had just made Copper using the reaction Al+CuSO4. I filtered the solution and let it dry overnight.
I decided to clean this Cu powder using 32.45% Tech grade HCl. Almost instantly, a white precipitate formed as the HCl went in.
This was definitely Copper (I) Chloride-- I had just been boiling Copper (II) Chloride with copper pennies being used as a reducing agent. After
making the Copper (I) Chloride, I shut off the other reaction since I had all the Cu(I)Cl I needed. I then added ammonia to the Copper Chloride and
bubbled Acetylene through it, making Copper Acetylide.
I tried to re-attempt this experiment with any variables I could imagine, but was unsuccessful. Can someone explain this?
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elementcollector1
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Quote: Originally posted by Camroc37  | So something I thought wasn't possible happened:
I had just made Copper using the reaction Al+CuSO4. I filtered the solution and let it dry overnight.
I decided to clean this Cu powder using 32.45% Tech grade HCl. Almost instantly, a white precipitate formed as the HCl went in.
This was definitely Copper (I) Chloride-- I had just been boiling Copper (II) Chloride with copper pennies being used as a reducing agent. After
making the Copper (I) Chloride, I shut off the other reaction since I had all the Cu(I)Cl I needed. I then added ammonia to the Copper Chloride and
bubbled Acetylene through it, making Copper Acetylide.
I tried to re-attempt this experiment with any variables I could imagine, but was unsuccessful. Can someone explain this? |
Why are you so sure the white powder was CuCl? Wiki describes it as "sparingly soluble in water, but very soluble in concentrated hydrochloric acid."
Therefore, if you added acid, you shouldn't be precipitating out any CuCl.
I'm also confused about your desired endproduct - you mentioned precipitating and cleaning copper, indicating that was what you wanted, but then used
the CuCl anyway?
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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Camroc37
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| Quote: Originally posted by elementcollector1 | | Quote: Originally posted by Camroc37 | So something I thought wasn't possible happened:
I had just made Copper using the reaction Al+CuSO4. I filtered the solution and let it dry overnight.
I decided to clean this Cu powder using 32.45% Tech grade HCl. Almost instantly, a white precipitate formed as the HCl went in.
This was definitely Copper (I) Chloride-- I had just been boiling Copper (II) Chloride with copper pennies being used as a reducing agent. After
making the Copper (I) Chloride, I shut off the other reaction since I had all the Cu(I)Cl I needed. I then added ammonia to the Copper Chloride and
bubbled Acetylene through it, making Copper Acetylide.
I tried to re-attempt this experiment with any variables I could imagine, but was unsuccessful. Can someone explain this? |
Why are you so sure the white powder was CuCl? Wiki describes it as "sparingly soluble in water, but very soluble in concentrated hydrochloric acid."
Therefore, if you added acid, you shouldn't be precipitating out any CuCl.
I'm also confused about your desired endproduct - you mentioned precipitating and cleaning copper, indicating that was what you wanted, but then used
the CuCl anyway? |
Sorry if that was confusing. The Cu(I)Cl I was making by reducing Cu(II)Cl was unneeded information. I only added a bit of HCl, about enough to cover
the copper. Sorry about not having measurements, I didn't expect this to happen. I was going to keep the copper, but decided to use it for making
Copper Acetylide when it magically turned to Cu(I)Cl. That's what it must be, I mean I succeeded in making Copper Acetylide...
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Orenousername
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Al + CuSO4 in aqueous solution? HCl can react with copper in the presence of H2O2 or some other oxidizer..
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Camroc37
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Posts: 101
Registered: 4-8-2015
Location: USA
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Mood: Must...Nitrate...EVERYTHING!
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Will try that
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