The reasons why copper dissolves in AgNO3 solution but remain insoluble in Pb(No3)2 solution.help me.thank you
See the activity series.
http://www.files.chem.vt.edu/RVGS/ACT/notes/activity_series.html
A metal will displace any ION BELOW it in the activity series.
Cu is ABOVE Ag but Cu is below Pb.
Cu + 2AgNO3 ==> Cu(NO3)2 + 2Ag
but
Cu + Pb(NO3)2 ==> No reaction because Cu is BELOW Pb in the series.
Solve simultaneously: 27 raise to power of x-y =9/3 raise to power of x,2 raise to power of x-2y =0.5.THANK YOU.
Your post will get lost here. You should post a new one at the top of the page and use the subject of math.
Copper dissolves in AgNO3 (silver nitrate) solution but remains insoluble in Pb(NO3)2 (lead nitrate) solution due to the difference in reactivity and the formation of different compounds.
To understand why this happens, we need to consider the reactions that occur between the metal (copper) and the respective nitrate solutions.
1. Copper and Silver Nitrate (AgNO3):
When copper is added to a solution of silver nitrate, a redox reaction takes place. Copper atoms undergo oxidation by losing electrons, while silver ions undergo reduction by gaining electrons. The overall reaction can be represented as:
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)
As a result, solid copper (Cu) dissolves in the silver nitrate solution, forming copper(II) nitrate (Cu(NO3)2) and silver (Ag) precipitates as a solid.
2. Copper and Lead Nitrate (Pb(NO3)2):
Unlike silver nitrate, lead nitrate lacks the oxidizing properties needed to oxidize copper. Therefore, when copper is added to a solution of lead nitrate, no redox reaction occurs. The reaction can be represented as:
Cu(s) + Pb(NO3)2(aq) → No reaction
Since the lead nitrate solution does not have the capability to oxidize copper, the copper remains insoluble, and no reaction takes place.
In summary, the different reactivity of silver nitrate and lead nitrate towards copper determines whether copper will dissolve or remain insoluble. Silver nitrate can oxidize copper, leading to a redox reaction that results in the dissolution of copper and the formation of silver precipitate. On the other hand, lead nitrate lacks oxidizing properties, so copper remains insoluble and no reaction occurs.