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The mole fraction of the solute in one molal aqueous solution is :-
A
0.027
B
0.036
C
0.018
D
0.009
Detailed Solution
A one molal solution contains 1 mole of solute in 1 kg (1000 g) of water.
Moles of water $= \dfrac{1000}{18} = 55.55$
Mole fraction of the solute $= \dfrac{n_{solute}}{n_{solute} + n_{water}} = \dfrac{1}{1 + 55.55}$
$= \dfrac{1}{56.55}$
$= 0.0177 \approx 0.018$
Moles of water $= \dfrac{1000}{18} = 55.55$
Mole fraction of the solute $= \dfrac{n_{solute}}{n_{solute} + n_{water}} = \dfrac{1}{1 + 55.55}$
$= \dfrac{1}{56.55}$
$= 0.0177 \approx 0.018$