Can copper sulphate solution be stored in an iron vessel? Explain.
Higher the standard reduction potential (Eº) value, greater the tendency of the species to accept electrons and undergo reduction.
Cu2++2e-→Cu, Eº = + 0.337 V ; Fe2+ + 2e- → Fe, Eº = - 0.440 V
Therefore, Cu2+ has a greater tendency to undergo reduction than Fe2+ or Fe can reduce (or displace) Cu2+ ions from its salt solution.
Fe(s) +Cu2(aq) → Fe2(aq) + Cu(s)
Hence, copper sulphate solution cannot be stored in an iron vessel as the iron vessel dissolves forming Fe2+ ions and Cu2+ ions from copper sulphate solution forms Cu.