Why does copper turnings dissolve in AgNo3 solution but remains soluble in PbNo3 solition

The activity series is for these three metals is as follows:

Pb ==> Pb^2+ + 2e
Cu ==> Cu^2+ + 2e
Ag ==> Ag^e + e
A metal ABOVE will dissolve and plate out an ION of a metal below. So Cu will go into solution (dissolve) and AgNO3 will deposit Ag metal. But Pb will stay as is and not dissolve in a Cu solution.
Cu is more easily oxidized (Cu ==> Cu^2+ + 2e) than Ag.

Did you know?

Did you know that copper turnings dissolve in AgNo3 (silver nitrate) solution but remain soluble in PbNo3 (lead nitrate) solution? This intriguing phenomenon is due to the reactivity of copper towards silver and lead. Copper is more reactive than silver, therefore, when copper turnings come into contact with AgNo3 solution, a redox reaction occurs between copper and silver ions. The copper atoms lose electrons, forming copper ions, while the silver ions gain those electrons and are reduced to solid silver. As a result, the copper turnings dissolve into the solution while solid silver precipitates out. On the other hand, copper is less reactive than lead, so it does not undergo the same reaction with PbNo3 solution. Therefore, copper turnings remain soluble in PbNo3 solution rather than forming a precipitate like in the case of AgNo3 solution. These differences in reactivity highlight the fascinating intricacies of chemical reactions and the behavior of different elements.