The mole fraction of solute in an aqueous solvent is 0.1. The molality of the solution is m.

Question

The mole fraction of solute in an aqueous solvent is 0.1. The molality of the solution is m. (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

x text solvent =1-x text solute =1-0.1=0.9 Assuming, moles of water =0.9 and moles of solute =0.1 Mass of water =0.9 × 18=16.20 g =0.0162 kg Molality =( text mol solute / text Mass of solvent ( kg )) =(0.1/0.0162)=6.17 m

Q. The mole fraction of solute in an aqueous solvent is $0.1$ . The molality of the solution is______ $m$ .

$x_{solvent} = 1 - x_{solute}$
$= 1 - 0.1 = 0.9$
Assuming, moles of water $= 0.9$ and moles of solute $= 0.1$
Mass of water $= 0.9 \times 18 = 16.20 g = 0.0162 k g$
Molality $= \frac{mol solute}{Mass of solvent ( k g )}$
$= \frac{0.1}{0.0162} = 6.17 m$

Q. The mole fraction of solute in an aqueous solvent is 0.1. The molality of the solution is______ m.

xsolvent ​=1−xsolute ​ =1−0.1=0.9 Assuming, moles of water =0.9 and moles of solute =0.1 Mass of water =0.9×18=16.20g=0.0162kg Molality = Mass of solvent (kg) mol solute ​ =0.01620.1​=6.17m

Q. The mole fraction of solute in an aqueous solvent is $0.1$ . The molality of the solution is______ $m$ .

$x_{solvent} = 1 - x_{solute}$
$= 1 - 0.1 = 0.9$
Assuming, moles of water $= 0.9$ and moles of solute $= 0.1$
Mass of water $= 0.9 \times 18 = 16.20 g = 0.0162 k g$
Molality $= \frac{mol solute}{Mass of solvent ( k g )}$
$= \frac{0.1}{0.0162} = 6.17 m$