You can find the molar conductivity of NaCl at infinite dilution (Λ°_NaCl) using the given conductivities of LiCl, NaNO₃, and LiNO₃ by applying Kohlrausch's Law.

Here's how:

Kohlrausch's Law states that the molar conductivity of a strong electrolyte at infinite dilution is the sum of the limiting ionic conductivities of its constituent ions.

Steps:

1. Identify the limiting ionic conductivities:

* Let Λ°_Li+ represent the limiting molar conductivity of the lithium ion (Li⁺).

* Let Λ°_Cl- represent the limiting molar conductivity of the chloride ion (Cl^-).

* Let Λ°_Na+ represent the limiting molar conductivity of the sodium ion (Na⁺).

* Let Λ°_NO3- represent the limiting molar conductivity of the nitrate ion (NO₃^-).

2. Write the equations for the given conductivities:

* Λ°_LiCl = Λ°_Li+ + Λ°_Cl-

* Λ°_NaNO3 = Λ°_Na+ + Λ°_NO3-

* Λ°_LiNO3 = Λ°_Li+ + Λ°_NO3-

3. Solve for the desired molar conductivity (Λ°_NaCl):

* Λ°_NaCl = Λ°_Na+ + Λ°_Cl-

4. Combine the equations to eliminate unwanted terms:

* Subtract the equation for Λ°_LiNO3 from the equation for Λ°_NaNO3 to get:

Λ°_NaNO3 - Λ°_LiNO3 = Λ°_Na+ - Λ°_Li+

* Add this result to the equation for Λ°_LiCl:

(Λ°_NaNO3 - Λ°_LiNO3) + Λ°_LiCl = Λ°_Na+ - Λ°_Li+ + Λ°_Li+ + Λ°_Cl-

* Simplify: Λ°_NaCl = Λ°_NaNO3 - Λ°_LiNO3 + Λ°_LiCl

Therefore, the molar conductivity of NaCl at infinite dilution (Λ°_NaCl) is equal to the sum of the molar conductivities of NaNO₃ and LiCl minus the molar conductivity of LiNO₃.

Important Note: This method relies on the assumption that all the electrolytes are strong electrolytes, meaning they fully dissociate into ions in solution.