How Do Metals React with Solutions of Other Metal Salts Class 10

Metals react with solutions of other metal salts through displacement reactions, where a more reactive metal displaces a less reactive metal from its salt solution. This reaction type follows the activity series: metals higher in the series can push out metals lower down. For instance, when an iron nail is placed in copper sulfate solution, iron displaces copper because iron is more reactive, forming iron sulfate in solution while copper metal precipitates out. The blue color of copper sulfate fades, and a reddish-brown coating of copper appears on the iron nail—a visual confirmation of the displacement.

The general pattern for these reactions is: Metal A + Salt of Metal B → Salt of Metal A + Metal B (only if A is more reactive than B). Common classroom demonstrations include zinc displacing copper from copper sulfate (turning the solution colorless while copper deposits form), or magnesium displacing zinc from zinc sulfate. These reactions are redox processes where the more reactive metal loses electrons (oxidation) while the metal ions in solution gain electrons (reduction). Understanding these displacement reactions helps students predict reaction outcomes, explain electroplating processes, and grasp fundamental concepts about electron transfer and chemical reactivity that appear throughout chemistry, from corrosion prevention to battery technology.