A student analyzes the purity of a solid mixture containing \(\text{NaCl}\) and an inert, water-soluble non-chloride impurity. The student dissolves a \(2.00 \text{ g}\) sample of the mixture completely in distilled water and adds an excess of \(1.0 \text{ M } \text{AgNO}_3\text{(aq)}\), precipitating all chloride ions as \(\text{AgCl(s)}\). The precipitate is filtered, washed, and dried to a constant mass of \(1.43 \text{ g}\). Given that the molar mass of \(\text{AgCl}\) is \(143.4 \text{ g/mol}\) and the molar mass of \(\text{NaCl}\) is \(58.4 \text{ g/mol}\), what is the percent by mass of \(\text{NaCl}\) in the original sample?