the colour of the solution observed after about 1 hour of placing iron nail in copper sulphate solution is
What is the color of the solution after placing an iron nail in copper sulfate solution for about one hour?
Answer: The reaction you are referring to involves a classic example of a displacement reaction. Here’s how it unfolds:
-
Initial Setup:
- You start with a blue solution, which is the color of copper sulfate ((CuSO_4)) in water. The blue color is due to the presence of (Cu^{2+}) ions in the solution.
-
Reaction Process:
- When an iron nail ((Fe)) is immersed in the copper sulfate solution, a displacement reaction occurs. Iron, being more reactive than copper, displaces copper from the sulfate compound.
The chemical equation for this reaction is as follows:
Fe(s) + CuSO_4(aq) \rightarrow FeSO_4(aq) + Cu(s)In this equation, solid iron (Fe) reacts with copper sulfate ((CuSO_4)), resulting in the formation of ferrous sulfate ((FeSO_4)) and copper metal (Cu).
-
Color Change Observation:
- As the reaction progresses, the color of the solution changes from blue to green. This color change is attributed to the formation of ferrous sulfate ((FeSO_4)), which imparts a pale green to light green color to the solution, depending on the concentration of the (Fe^{2+}) ions in the solution.
-
Formation of Copper:
- Concurrently, copper metal is deposited on the surface of the iron nail. You might observe reddish-brown copper particles forming on the nail.
In conclusion, after approximately one hour, the distinctive blue color of the copper sulfate solution is replaced by a green color due to the formation of ferrous sulfate, accompanied by the deposition of copper on the iron nail. This observable change effectively demonstrates the reactivity of iron in displacing copper from its compound.
If there are any additional queries or if you’re conducting a related experiment and need further clarification, feel free to ask! @username