A sample of `Mg` was burnt in air to give a mixure of `MgO` and `Mg_(3)N_(2)`. The ash was dissolved in `60 Meq`. of `HCl` and the resulting solution was back titrated with `NaOH`. `12 Meq`. Of `NaOH` was then added and the solution distrilled. The ammonia released was then trapped in `10 Meq`. of second acid solution. Back titration of this solution required `6 Meq`. of the base Calculate the percentage of `Mg` burnt to the nitride.

Explanation

To solve the problem, we need to calculate the percentage of magnesium (Mg) that was burnt to form magnesium nitride (Mg3N2) from the given data. We will follow these steps:

### Step 1: Define Variables
Let:
- \( A \) = moles of Mg used to form MgO
- \( B \) = moles of Mg used to form Mg3N2

### Step 2: Write the Reactions
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