Question #44532

A $2.665 \text{ g}$ sample of a mixture containing two hydrate isomers of $\ce{CrCl3 \cdot 6H2O}$, Isomer X (pale green) and Isomer Y (dark green), is dissolved in $100 \text{ g}$ of water at $298 \text{ K}$. The boiling point of this solution is found to be $100.1456^\circ\text{C}$ at $1 \text{ atm}$. If the entire solution is treated with excess $\ce{AgNO3(aq)}$, what mass of $\ce{AgCl(s)}$ will precipitate?

(Assume the boiling point of pure water is $100.000^\circ\text{C}$ at $1 \text{ atm}$, $100\%$ ionization of the complex salts, ideal behavior, and no aquation of the inner coordination sphere. Given: $K_b(\ce{H2O}) = 0.52 \text{ K kg mol}^{-1}$, Molar mass of $\ce{CrCl3 \cdot 6H2O} = 266.5 \text{ g mol}^{-1}$, Molar mass of $\ce{AgCl} = 143.5 \text{ g mol}^{-1}$)