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 different metal vessels (zinc, silver, and gold), we will analyze the standard electrode potentials of the metals involved.

### Step-by-Step Solution:

**Step 1: Analyze Copper Sulfate and Zinc Vessel**
- Given:
- Standard electrode potential of \( Cu^{2+}/Cu = +0.34 \, V \)
- Standard electrode potential of \( Zn^{2+}/Zn = -0.76 \, V \)
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