Ash96 - 17-11-2012 at 07:06
if i add CuO or CuCO3 or CuCl2 to sulphuric acid will i get CuSO4 ?
Random - 17-11-2012 at 07:20
yes if homework question
yet calcined CuO may have hard time reacting and CuCl2 would create a mixture of unwanted ions
Ash96 - 17-11-2012 at 07:40
so i can add CuO or CuCO3 in hot concentrated sulfuric acid right ?
[Edited on 17-11-2012 by Ash96]
Random - 17-11-2012 at 08:14
If I wanted to prepare CuSO4 I would use like 35- 50% sulfuric acid at room temp with CuCO3 until no more CuCO3 reacts, then filter and evaporate the
solution
ElectroWin - 17-11-2012 at 11:45
yes, i have done this.
i used hot conc H2SO4 to attack native copper, then make CuSO4, as follows:
H2SO4 + Cu --> CuO + SO2 + H2O
H2SO4 + CuO --> CuSO4 + H2O
the result was a mixture of anhydrous CuSO4 with the monohydrate and CuO.
i purified by dissolving in water and recrystallized; and
the CuO was recycled back to make more CuSO4.
Hexavalent - 17-11-2012 at 13:08
Electrolysis of copper in sulfuric acid works well for me when I need more copper sulfate on the fly, as I have a fair amount of technical sulfuric
acid and copper. I also like it due to its ease: I set it up, cover it and leave it sit for a few hours. Et voila, copper sulfate. I usually
recrystallize after making it to maximize purity, and one can get some very nice blue crystals from it.
bfesser - 17-11-2012 at 14:52
Copper(II) oxide will react with concentrated sulfuric acid, generating aqueous copper(II) sulfate, as shown:
CuO<em>(s.)</em> + H<sub>2</sub>SO<sub>4</sub><em>(aq.)</em> →
CuSO<sub>4</sub><em>(aq.)</em> + H<sub>2</sub>O<em>(l.)</em>
Copper(II) carbonate will react with sulfuric acid, generating copper(II) sulfate, as shown:
CuCO<sub>3</sub><em>(s.)</em> + H<sub>2</sub>SO<sub>4</sub><em>(aq.)</em> →
CuSO<sub>4</sub><em>(aq.)</em> + H<sub>2</sub>O<em>(l.)</em> +
CO<sub>2</sub><em>(g.)</em>
Copper(II) chloride may react with concentrated sulfuric acid, liberating hydrogen chloride gas, as shown:
CuCl<sub>2</sub><em>(s.)</em> + H<sub>2</sub>SO<sub>4</sub><em>(aq.)</em> →
CuSO<sub>4</sub><em>(aq.)</em> + 2 HCl<em>(g.)</em>
Avoid using the chloride, as the resulting solution (or first crop of crystals) will invariably contain trace hydrogen and chloride ions, and the
hydrogen chloride gas will hydrate and dissolve your lungs.
bfesser - 19-11-2012 at 08:57
Oh, forgot to mention that concentrated sulfuric acid will dehydrate copper(II) sulfate pentahydrate to anhydrous copper(II) sulfate.