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Can we store copper sulphate solution in...

Can we store copper sulphate solution in iron vessel? Give suitable explanation in support of your answer
`[E°(Cu^(2+)//Cu)=+0.34V,E°(Fe^(2+)//Fe)=-0.44V]`

Text Solution

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Let us see if copper sulphate reacts with iron or not if it reacts, then copper sulphate cannot be stored in iron vessel.
Iron will react (if possible) with copper sulphate, as follows:
`Fe(s)+CuSO_(4)(aq) to FeSO_(4)(aq)+Cu(s)`
Or `Fe(s)+Cu^(2+)(aq) to Fe^(2+)(aq)+Cu(s)`
The two half cell reactions are as follows:
`Fe(s) to Fe^(2+)(aq)+2e^(-)`
`Cu^(2+)(aq)+2e^(-) to Cu(s)`
The cell representing this redox reaction is:
`Fe|Fe^(2+)(aq)||Cu^(2+)|Cu` ,br> `EMF^(@)=E_(Cu^(2+)//Cu)^(@)-E_(Fe^(2+)//Fe)^(@)`
`=+0.34V-(-0.44V)`
`=(0.34+0.44)V=0.78V`
As the `EMF^(@) gt0`, the reaction is spontaneous in the given direction. thus copper sulphate cannot be stored in iron vessel.
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