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Question
Can copper sulphate solution be stored in an iron vessel? Explain.
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Solution
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.
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