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How do you make copper acetate?
I am using vinegar and salt-then adding bits of copper to solution.
Have tried running a current through it-however the copper wires I use get corroded very quickly.
Thanks alot
Lancenigo di Villorba (TV), Italy
Don't worry, copper may corrode in vinegar!
ABOUT YOUR REMARKS
I understood not what SALT you said about it.
On the other hand, you made copper corrosion by means of standing copper bits or wires in vinegar added of a salt.
Surely, a quicker process may be an acid-base reaction when you can put copper carbonate or other basic compounds of copper. Instead, it is not simply find them, indeed the most common copper's compound is sulphate's blue crystals.
MY REMARKS
1st WAY)
I remember you that air's oxygen is an oxidizer able to corrode copper in acidic media, thus you needs only a continuous air's uptaking in the acidic mixture.
Electrochemical half-reactions are written here below :
-) Cu(s) ---> Cu++(aq) + 2e (+0.34 V)
-) O2(g) + 4 CH3COOH(aq) + 4e --->
---> 4 CH3COO-(aq) + 2 H2O(aq) (+0.95 V instead 1.22)
As you see, the former electrical potential is lower than the second one, thus the corrosion phenomena NEED NOT a voltaic battery. Moreover, the second electrical potential is corrected on basis of presence of acetic acid.
2nd WAY)
You made right, a faster feature involves electrochemical applications. You put two rods in vinegar, one copper's rod and one graphite's one. An external electrical energy source (e.g. voltaic battery) is connected to two rods by means of conductor wires. You can see a fast coloration of the medium in greenish hue.
Electrochemical half-reactions are written here below :
-) Cu(s) ---> Cu++(aq) + 2e (+0.34 V)
-) 2 CH3COOH(aq) + 2e --->
---> 2 CH3COO-(aq) + H2(g) (-0.27 V instead 0.00)
As you see, the former electrical potential is greater than the second one, thus the corrosion phenomena NEED a voltaic battery. Moreover, the second electrical potential is corrected on basis of presence of acetic acid.
3rd WAY)
Another feature permits you a fast process, this involves oxidizer stuff. You put copper's bits in vinegar and you add several drops of hydrogen peroxide. By means of a gentle and continuous medium's warming you can see a fast coloration of the medium in greenish hue.
Electrochemical half-reactions are written here below :
-) Cu(s) ---> Cu++(aq) + 2e (+0.34 V)
-) H2O2(g) + 2 CH3COOH(aq) + 2e --->
---> 2 CH3COO-(aq) + 2 H2O(aq) (+1.50 V instead +1.77)
As you see, the former electrical potential is lower than the second one, thus the corrosion phenomena NEED NOT a voltaic battery. Moreover, the second electrical potential is corrected on basis of presence of acetic acid.
I hope this helps you.
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