How do we prepare copper(II) nitrate?

Question

I googled it but could not find relevant results.

I really need help in the detailed procedure. A link that contains the preparation of copper(II) nitrate will do as well.

thanks.

Answer 1

Submerse Cu(s) in AgNO3 ( silver nitrate solution ).
Wait for the chemical reaction and you will see Ag forming on the outside of the copper and replacing it, you now have 2 Ag on the exposed area of the copper.
The copper is replacing the silver in silver nitrate.
This reaction is a single-replacement reaction.
Balanced equation is :
Cu(s) + 2 AgNO3 >> 2 Ag(s) + Cu(NO3)2

Answer 2

Funny I found this question because I just got done making this stuff lol. Dissolve as much ammonium nitrate in water as possible. Hook two thick copper wires to a 12 volt battery( for fast and larger quantity of production) and perform electrolosis by placing the wires in the solution. Watch the wire b/c you may have to replace it often when the reaction eats up the copper. You should smell ammonia as the ammonium ion breaks apart and is replaced by a copper atom. after awhile the solution should be very dark blue. filter the solution. There will be a light blue powder in the bottom of the container where the reaction took place, this is copper hydroxide(weak base) u may want to save this because it can be reacted with nitric acid to form Copper Nitrate as well(more dangerous). The solution can be left out in the sun and dark blue crystals will form in a couple days.

Reaction
NH4NO3+Cu=Cu(NO3)2+NH3+4H
I think this is right, but you might have to add into the equation the water.

Answer 3

the regulation of conservation of mass is purely because it variety of feels, it extremely is that mass can neither be formed or created and remains consistent in a closed equipment. This chemicl reaction is a closed equipment. The preliminary mass of fabric with be equivalent to the purely suitable mass. As silver nitrate is a precipitate and exceedingly much insoluble the reaction is exceedingly complete. 6.8+2.4= 9.2g to start up with. 3.4 + x = 9.2g to end. purely calculate how many grams is X

Answer 4

Steve is correct....but do it in a well ventilated area and don't breathe the red gas produced.

Answer 5

Dissolve Cu metal in con. HNO3. That info may improve your searching.