Given `:`
`E^(c-)._(Ag^(o+)|Ag)=0.80V, E^(c-)._(Mg^(2+)|Mg)=-2.37V,`
`E^(c-)._(Cu^(2+)|Cu)=0.34V,E^(c-)._(Hg^(2+)|Hg)=0.79V`
Which of the following statements is `//` are incorrect ?

Options

A. `AgNO_(3)` can be stored in copper vessel.
B. `Cu(NO_(3))_(2)` can be stored in copper vessel.
C. `CuCl_(2)` can be stored in silver vessel.
D. `HgCl_(2)` can be stored in copper vessel.

Explanation

To solve the problem, we need to analyze the given standard reduction potentials and determine the feasibility of storing different compounds in specified vessels based on their electrochemical reactions. Here’s a step-by-step solution:

### Step 1: Understand the Standard Reduction Potentials
We are given the following standard reduction potentials:
- \( E^\circ(Ag^+|Ag) = +0.80 \, V \)
- \( E^\circ(Mg^{2+}|Mg) = -2.37 \, V \)
- \( E^\circ(Cu^{2+}|Cu) = +0.34 \, V \)
- \( E^\circ(Hg^{2+}|Hg) = +0.79 \, V \)

### Step 2: Analyze Each Statement
We need to determine whether the statements regarding the storage of different compounds in specific vessels are correct or incorrect.

#### Statement A: Silver nitrate can be stored in a copper vessel.
- **Reaction**: \( Ag^+ + Cu \rightarrow Ag + Cu^{2+} \)
- **Cell Potential Calculation**:
\[ E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} = 0.80 - 0.34 = 0.46 \, V \]
- Since \( E^\circ_{cell} > 0 \), the reaction is spontaneous. Thus, **this statement is incorrect**.

#### Statement B: Copper nitrate can be stored in a copper vessel.
- **Reaction**: \( Cu^{2+} + Mg \rightarrow Cu + Mg^{2+} \)
- **Cell Potential Calculation**:
\[ E^\circ_{cell} = 0.34 - (-2.37) = 0.34 + 2.37 = 2.71 \, V \]
- Since \( E^\circ_{cell} > 0 \), the reaction is spontaneous. Thus, **this statement is incorrect**.

#### Statement C: Cuprous chloride can be stored in a silver vessel.
- **Reaction**: \( Cu^+ + 2Ag \rightarrow Cu + 2Ag^+ \)
- **Cell Potential Calculation**:
\[ E^\circ_{cell} = 0.34 - 0.80 = -0.46 \, V \]
- Since \( E^\circ_{cell} < 0 \), the reaction is not spontaneous. Thus, **this statement is correct**.

#### Statement D: Mercury chloride can be stored in a copper vessel.
- **Reaction**: \( Hg^{2+} + Cu \rightarrow Hg + Cu^{2+} \)
- **Cell Potential Calculation**:
\[ E^\circ_{cell} = 0.79 - 0.34 = 0.45 \, V \]
- Since \( E^\circ_{cell} > 0 \), the reaction is spontaneous. Thus, **this statement is incorrect**.

### Conclusion
The incorrect statements are:
- **Statement A**: Silver nitrate cannot be stored in a copper vessel.
- **Statement B**: Copper nitrate cannot be stored in a copper vessel.
- **Statement D**: Mercury chloride cannot be stored in a copper vessel.

### Final Answer
The incorrect statements are A, B, and D.