The blue colour of aqueous copper sulphate solution can be changed to pale green by immersing which of the following metal rod in it?
(a) Iron
(b) Zinc
(c) Aluminium
(d) Silver
Answers
Answer :
Iron. The blue colour of aqueous copper sulphate solution can be changed to place green by immersing an iron rod in it.
Explanation :
Out of the given options, all except silver can displace copper from its solution. But, we are also asked that the solution should be changed to a colour of pale-green. Hence, the answer is iron beacuse the colour of iron sulphate solution is pale-green.
When an iron rod is immersed in the copper sulphate solution it displaces copper from its solution and forms iron sulphate solution which gives a pale green colour to the resultant solution.
Reaction :
_____________
Additional Information :
Displacement reaction :
A type of chemical reaction in which an atom or group of atoms displace another atom or group of atoms of a compound. Displacement reactions are also called single-displacement reactions.
Examples :
Answer:
nswer :
Iron. The blue colour of aqueous copper sulphate solution can be changed to place green by immersing an iron rod in it.
Explanation :
Out of the given options, all except silver can displace copper from its solution. But, we are also asked that the solution should be changed to a colour of pale-green. Hence, the answer is iron beacuse the colour of iron sulphate solution is pale-green.
When an iron rod is immersed in the copper sulphate solution it displaces copper from its solution and forms iron sulphate solution which gives a pale green colour to the resultant solution.
Reaction :
\sf{CuSO_4(aq)+Fe(s)\longrightarrow{}\underset{\textsf{pale green}}{FeSO_4(aq)}+Cu(s)}CuSO4(aq)+Fe(s)⟶pale greenFeSO4(aq)+Cu(s)
_____________
Additional Information :
Displacement reaction :
A type of chemical reaction in which an atom or group of atoms displace another atom or group of atoms of a compound. Displacement reactions are also called single-displacement reactions.
Examples :
\sf{CuCl_2(aq)+Zn(s)\longrightarrow{}ZnCl_2(aq)+Cu(s)}CuCl2(aq)+Zn(s)⟶ZnCl2(aq)+Cu(s)
\sf{CuSO_4(aq)+Zn(s)\longrightarrow{}ZnSO_4(aq)+Cu(s)}CuSO4(aq)+Zn(s)⟶ZnSO4(aq)+Cu(s)
\sf{CuCl_2(aq)+Pb(s)\longrightarrow{}PbCl_2(aq)+Cu(s)}CuCl2(aq)+Pb(s)⟶PbCl2(aq)+Cu(s)