A 2.00 g solid mixture contains only $\mathrm{NaCl}$ and $\mathrm{NaBr}$, with $\mathrm{NaCl}$ forming 35.0% of the mass. The mixture is dissolved in water and treated with excess $\mathrm{AgNO}{}_3$ solution. The precipitate is shaken with excess dilute aqueous ammonia, which dissolves all the $\mathrm{AgCl}$ (assume $\mathrm{AgBr}$ stays completely undissolved), and then filtered. Find the mass of the undissolved residue in grams, to two decimal places. (Na 23, Cl 35.5, Br 80, Ag 108.)

Numerical answer type, answer in g, tolerance 0.01.