Calculate the molar conductivity of a solution of `MgCl_(2)` at infinte dilution given that the molar ionic conductivities of `lambda^(@) (Mg^(2+)) = 106.1 S cm^(2) mol^(-1)` and `lambda^(@) (Cl^(-)) = 76.3 S cm^(2) mol^(-1)`

Explanation

To calculate the molar conductivity of a solution of \( \text{MgCl}_2 \) at infinite dilution, we can use Kohlrausch's law of independent migration of ions. The law states that the molar conductivity of an electrolyte at infinite dilution can be expressed as the sum of the molar ionic conductivities of its constituent ions.

### Step-by-Step Solution:

1. **Identify the dissociation of \( \text{MgCl}_2 \)**:
\[ \text{MgCl}_2 \rightarrow \text{Mg}^{2+} + 2 \text{Cl}^- \]
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