Why can't we store AgNO3 solution in copper vessel ?

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Solution

We cannot store silver nitrate, AgNO₃ solution in copper vessel because according to reactivity series copper is more reactive than silver. Thus it will displace silver from AgNO₃solution forming copper nitrate soltuion. The reaction is:
2AgNO₃(aq) + Cu(s) $\to$ Cu(NO₃)₂(aq) + 2Ag(s)

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We cannot store $CuSO_4$ solution in an iron vessel. Why?

Copper solutions are stored in iron vessels.

Q. Given

E_{A g^{+} / A g}^{0} = 0.80 V, E_{M g^{2 +} / M g}^{0} = - 2.372 V, E_{C u^{2 +} / C u}^{0} = 0.34 V, E_{H g^{2 +} / H g}^{0} = 0.79 V

Which of the following statement(s) is/are correct?

Given:
$E_{A g^{+} / A g}^{0} = 0.80 V$ ,
$E_{M g^{2 +} / M g}^{0} = - 2.37 V$ ,
$E_{C u^{2 +} / C u}^{0} = 0.34 V$ ,
$E_{H g^{2 +} / H g}^{0} = 0.79 V$
Which of the following statements is/are correct ?

Q. Can we store copper sulphate in iron container and why?

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Why can't we store AgNO3 solution in copper vessel ?

We cannot store silver nitrate, AgNO3 solution in copper vessel because according to reactivity series copper is more reactive than silver. Thus it will displace silver from AgNO3 solution forming copper nitrate soltuion. The reaction is: 2AgNO3(aq) + Cu(s) →Cu(NO3​)2(aq)​ + 2Ag(s)

We cannot store silver nitrate, AgNO₃ solution in copper vessel because according to reactivity series copper is more reactive than silver. Thus it will displace silver from AgNO₃solution forming copper nitrate soltuion. The reaction is:
2AgNO₃(aq) + Cu(s) $\to$ Cu(NO₃)₂(aq) + 2Ag(s)