Total number of moles of `EDTA^(4-)` required to produce octahedral complex with `Mg^(2+)` is

Explanation

To determine the total number of moles of `EDTA^(4-)` required to produce an octahedral complex with `Mg^(2+)`, we can follow these steps:

### Step 1: Understand the Coordination Number
In an octahedral complex, the coordination number is 6. This means that a central metal ion can be surrounded by 6 ligands.

**Hint:** Remember that the coordination number indicates how many ligands can bond to the central metal ion.

### Step 2: Identify the Type of Ligand
`EDTA^(4-)` is a hexadentate ligand, which means it can form six bonds with a metal ion. This property makes it suitable for forming octahedral complexes.

**Hint:** Hexadentate ligands can bind to a metal ion at six different sites.

### Step 3: Determine the Metal Ion
In this case, the metal ion is `Mg^(2+)`. When `EDTA^(4-)` coordinates with `Mg^(2+)`, it will form a complex.

**Hint:** The charge of the metal ion and the ligand can affect the overall charge of the complex formed.

### Step 4: Calculate the Number of Moles of EDTA Required
Since one `EDTA^(4-)` can coordinate with `Mg^(2+)` to form a complex with a coordination number of 6, only one mole of `EDTA^(4-)` is required to form the octahedral complex.

**Hint:** For each octahedral complex, consider how many ligands are needed based on the coordination number.

### Conclusion
Therefore, the total number of moles of `EDTA^(4-)` required to produce an octahedral complex with `Mg^(2+)` is **1 mole**.

**Final Answer:** 1 mole of `EDTA^(4-)` is required.