An unknown non-electrolyte compound has a molecular weight of 180 g/mol. When 1.8 g of this compound is dissolved in 100 g of water, the freezing point of the solution is found to be $-0.186^{\circ}\text{C}$. Given that the cryoscopic constant ($K_f$) for water is $1.86^{\circ}\text{C kg/mol}$.
What is the van't Hoff factor ($i$) for a 0.05 m solution of sodium chloride (NaCl) that exhibits the same freezing point depression under identical conditions? Assume ideal behavior for NaCl solution.