Reaction:
* Silver nitrate (AgNO₃), a colorless solution, reacts with iron (Fe), a solid metal.
* The more reactive iron displaces the less reactive silver from the silver nitrate solution.
* Iron(II) nitrate (Fe(NO₃)₂) , a greenish solution, is formed.
* Silver (Ag), a solid metal, is deposited out of the solution as a grayish-white precipitate.
Equation:
2 AgNO₃(aq) + Fe(s) → Fe(NO₃)₂(aq) + 2 Ag(s)
Observations:
* You will observe a grayish-white precipitate forming on the surface of the iron metal.
* The solution will turn from colorless to greenish.
* The iron metal will start to dissolve.
Explanation:
This reaction occurs because iron is more reactive than silver on the reactivity series of metals. This means iron has a stronger tendency to lose electrons and form positive ions. In the reaction, iron atoms lose electrons to form Fe²⁺ ions, while silver ions (Ag⁺) in the solution gain electrons and become silver atoms.
Note:
* The reaction can be sped up by heating the solution or by using a more concentrated solution of silver nitrate.
* The reaction can be used to produce silver metal from silver nitrate solutions.
* This reaction is also a good example of a redox reaction, where electrons are transferred from iron to silver.
