When I made copper (II) citrate it stayed in solution and was a real pain to dry. It would form a syrup and take forever to get any drier. I love the colour of copper (II) acetate.
copper citrate will sometimes complex with concentrated citrate (mostly under basic conditions), so more dilute might actually work better! Warming the solution up can also encourage it to precipitate.
+vibzz lab Actually the correct formula for the basic copper carbonate that you prepared is Cu2(OH)2CO3. And this is the rection equation: 2 CuSO4 + 2 Na2CO3 + H2O = Cu2(OH)2CO3 + 2 Na2SO4 + CO2.
Nice vid! However there is an easier way to prepare the compound. You use the same amount of chemicals but first mix the Na2CO3 with the Citric acid dissolved in as little water as you need to dissolve it. Then, you add a fairly concentrated solution of the copper sulfate and stir it around. A very beautiful dark blueish green solution should have formed. From this point, you have two options. Option one is to let the solution sit for a day to precipitate the copper citrate. Option two is to heat up the solution until boiling for about 5 minutes, however I do not recommend this method because the sudden boiling really tends to bump the beaker around so that the solution gets boiled out of the beaker. Google superheating and you should know I mean. The copper citrate can then be filtered, washed and dried
That is a very interesting reaction. I did not imagine that copper citrate would decompose to copper powder and CO2 on heating, but yes, citrate acts is a reducing agent, being an antioxidant.
Excelent video!!!😊 Dear friend, could you tell me what other compounds result from the pyrolytic decomposition of copper citrate, in addition to pyrophoric copper? Thanks!
Copper Sulfate and Sodium Carbonate undergo a reaction to form Sodiu Sulfate and Copper carbonate. The sodium sulfate is removed as it's soluble in water. Copper carbonate is precipitated. It's then allowed to react with citric acid to form a solution of copper citrate. It doesn't have sulfate as we removed it as sodium sulfate
Cool! I only did know the experiment with pyrophoric Iron from Iron oxalate before. Would this also work with Acetic Acid instead of Citric Acid, so you get Copper Acetate?
The "copper citrate" may be a rather complicated compound . Check en.wikipedia.org/wiki/Iron(II)_citrate . One suspicious clue is the sudden change from a blue clear solution to a precipitate in an apparently colorless solution It seems to have been triggered by an increase of the Cu/citrate ratio or pH. At the very least, the former may have contained mostly dihydrogen citrate or hydrogen citrate anions, whereas the final stoichometric product had mostly citrate. Since citrate has three carboxylate "heads", and each copper will want to connect to two of them, an insoluble polymer is not unexpected. See iron(II) and colbalt oxalates.Each oxalate has two caboxylate heads, and each metal atom attaches to two of them, but not from the same anion; the result is an insoluble linear polymer...
Yes, it's basic copper carbonate and it is important. I think that equation of reaction between copper sulfate and sodium carbonate should look like 2 Na2CO3 + 2 CuSO4 -> CuCO3 • Cu(OH)2 + CO2 + 2 Na2SO4 And that is why it foams so much
Nice, I love this stuff! I usually make it from a basic citrate salt (like trisodium) and copper sulfate, since they are both soluble the product is easier to isolate & purify, and precipitation drives the reaction forwards. Also, you can buy basic citrate OTC in relative bulk for not much money: ruclips.net/video/PTp0yf_Wgk8/видео.html Your shot of the pyrophoria was better than any I'd been able to get, good job!
When I made copper (II) citrate it stayed in solution and was a real pain to dry. It would form a syrup and take forever to get any drier.
I love the colour of copper (II) acetate.
copper citrate will sometimes complex with concentrated citrate (mostly under basic conditions), so more dilute might actually work better! Warming the solution up can also encourage it to precipitate.
+vibzz lab Actually the correct formula for the basic copper carbonate that you prepared is Cu2(OH)2CO3.
And this is the rection equation: 2 CuSO4 + 2 Na2CO3 + H2O = Cu2(OH)2CO3 + 2 Na2SO4 + CO2.
Fantastic video! I loved the demonstration at the end.
Fantastic. Can you please elaborate to prepare magnesium citrate, calcium citrate and zinc citrate in detail for supplementation.
Nice vid! However there is an easier way to prepare the compound. You use the same amount of chemicals but first mix the Na2CO3 with the Citric acid dissolved in as little water as you need to dissolve it. Then, you add a fairly concentrated solution of the copper sulfate and stir it around. A very beautiful dark blueish green solution should have formed. From this point, you have two options. Option one is to let the solution sit for a day to precipitate the copper citrate. Option two is to heat up the solution until boiling for about 5 minutes, however I do not recommend this method because the sudden boiling really tends to bump the beaker around so that the solution gets boiled out of the beaker. Google superheating and you should know I mean. The copper citrate can then be filtered, washed and dried
That is a very interesting reaction. I did not imagine that copper citrate would decompose to copper powder and CO2 on heating, but yes, citrate acts is a reducing agent, being an antioxidant.
After the copper II citrate is heated and cooled down completley, will it still get red hot as it reacts with the oxygen in the air? I think not.
Maybe you are right, I am not sure, but at least it works with pyrophoric Iron, even if cooled down.
Excelent video!!!😊
Dear friend, could you tell me what other compounds result from the pyrolytic decomposition of copper citrate, in addition to pyrophoric copper?
Thanks!
Is this flash copper for plating steel
Simple and fun! I presume this provides a good path to a copper oxide catalyst with lots of surface area.
Will Copper sulfate and sodium citrate work to produce the same product.
Where does the sulfate go. Is it stil in there? I only know how to make copper citrate with electrolyse. And its a tedious process with low yield.
Copper Sulfate and Sodium Carbonate undergo a reaction to form Sodiu Sulfate and Copper carbonate. The sodium sulfate is removed as it's soluble in water. Copper carbonate is precipitated. It's then allowed to react with citric acid to form a solution of copper citrate. It doesn't have sulfate as we removed it as sodium sulfate
Cool! I only did know the experiment with pyrophoric Iron from Iron oxalate before.
Would this also work with Acetic Acid instead of Citric Acid, so you get Copper Acetate?
Nope. It doesn't work
make videos on photochemical reactions of compounds too
Nice Information
Thank you so much
Lead(II) citrate can also form pyrophoric lead
@@vibzzlab i think you have watched the video of lab lulz on thermal decomposition of copper citrate
@@vibzzlab hmm
@@vibzzlab pls watch mine too
The "copper citrate" may be a rather complicated compound . Check en.wikipedia.org/wiki/Iron(II)_citrate .
One suspicious clue is the sudden change from a blue clear solution to a precipitate in an apparently colorless solution It seems to have been triggered by an increase of the Cu/citrate ratio or pH.
At the very least, the former may have contained mostly dihydrogen citrate or hydrogen citrate anions, whereas the final stoichometric product had mostly citrate.
Since citrate has three carboxylate "heads", and each copper will want to connect to two of them, an insoluble polymer is not unexpected.
See iron(II) and colbalt oxalates.Each oxalate has two caboxylate heads, and each metal atom attaches to two of them, but not from the same anion; the result is an insoluble linear polymer...
Oh cool😍
You might wanna try pyrophoric iron too😁
Nice video. Actually That is Basic copper carbonate not copper carbonate. I'm also working on pyrophoric nickel experiments these days.
Yes, it's basic copper carbonate and it is important. I think that equation of reaction between copper sulfate and sodium carbonate should look like
2 Na2CO3 + 2 CuSO4 -> CuCO3 • Cu(OH)2 + CO2 + 2 Na2SO4
And that is why it foams so much
Nice content 👌
Make anti iron chemical for copper pot
Nice, I love this stuff! I usually make it from a basic citrate salt (like trisodium) and copper sulfate, since they are both soluble the product is easier to isolate & purify, and precipitation drives the reaction forwards. Also, you can buy basic citrate OTC in relative bulk for not much money:
ruclips.net/video/PTp0yf_Wgk8/видео.html
Your shot of the pyrophoria was better than any I'd been able to get, good job!