Is it possible to store:
(i) Copper sulphate solution in a zinc vessel?
(ii) Copper sulphate solution in a silver vessel?
(iii) Copper sulphate solution in a gold vessel?
Given: `E_(Cu^(2+)| Cu )^(0)` = + 0.34 volt and `E_(Ag^(2+)| Ag )^(0)` = 0.80 volt and `E_(Au^(2+)| Au )^(0)` = +1.50 volt

Explanation

To determine whether it is possible to store copper sulfate solution in zinc, silver, and gold vessels, we will analyze the standard reduction potentials provided for copper, silver, and gold, and compare them with zinc.

### Step-by-Step Solution:

**Step 1: Understanding Standard Reduction Potentials**
- The standard reduction potential (E°) indicates the tendency of a species to gain electrons (be reduced). A higher E° value means a stronger oxidizing agent, while a lower E° value indicates a stronger reducing agent.
- Given values:
- \(E_{Cu^{2+}/Cu}^0 = +0.34 \, \text{V}\)
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