Data:
m (molality) = 0.950 mol/Kg
moles of solute = ? (mol) = ?
mass of solvent = 85.4 g → 0.0854 Kg
Formula:
\(m = \frac{moles\:of\:solute}{mass\:of\:solvent}\)
Solving:
\(m = \frac{moles\:of\:solute}{mass\:of\:solvent}\)
\(0.950\:mol/\diagup\!\!\!\!\!\!K\diagup\!\!\!\!\!\!g = \frac{moles\:of\:solute}{0.0854\:\diagup\!\!\!\!\!\!K\diagup\!\!\!\!\!\!g}\)
\(moles\:of\:solute = 0.950*0.0854\)
\(\boxed{\boxed{moles\:of\:solute = 0.08113 \approx 0.0811\:mol}}\) \(\end{array}}\qquad\quad\checkmark\)
Answer:
0.0811 mol
