Explanation:
As it is known that non-electrolytes do not dissociate. Therefore, molarity of such a solution is equal to the osmolarity of solution.
As, molar mass of ethanol = 46.07 g/mol
Therefore, no. of moles of ethanol will be calculated as follows.
No. of moles = [tex]\frac{mass}{\text{molar mass}}[/tex]
= [tex]\frac{0.00001 g}{46.07 g/mol}[/tex]
= [tex]2.17 \times 10^{-7}[/tex] mol
As, molarity is moles of solute in liter of solution. Hence, molarity of ethanol is as follows.
Molarity = [tex]\frac{\text{no. of moles}}{volume}[/tex]
= [tex]\frac{2.17 \times 10^{-7} mol}{1 L}[/tex]
= [tex]2.17 \times 10^{-7}[/tex] mol/L
Since, for the given solution Molarity = osmolarity
Thus, we can conclude that osmolarity of .00001 grams (0.1 mg%) of ethanol in 1 L is [tex]2.17 \times 10^{-7}[/tex] osmol/L.
