## Chemistry and Chemical Reactivity (9th Edition)

In 1 liter of solution: Number of moles of solute: $14.8\ mol/L\times 1\ L=14.8\ mol$ Mass of solute: $14.8\ mol\times 17.03\ g/mol=252.04\ g$ Mass of solution: $1000\ cm^3\times 0.90\ g/cm^3=900\ g$ Mass of solvent: $900-252.4=647.96\ g$ Number of moles of solvent: $647.96\ g\div 18.015\ g/mol=35.97\ mol$ Molality: $14.8\ mol\div 0.648\ kg=22.84\ m$ Weight percent: $252.04/900\times100\%=28\%$ Mole fraction: $14.8\div(14.8+35.97)=0.29$