A solution of glucose in water is labelled as `10 "percent" w//w`, what would be the molality and mole fraction of each component in the solution? If the density of the solution is `1.2 g mL^(-1)`, then what shall be the molarity of the solution?

Explanation

10 g glucose is present in 100 g solution, i.e., 90 g of water = 0.090 kg of water
`"10 g of glucose "=(10)/(180)" mol = 0.0555 mol, 90 g "H_(2)O=(90)/(18)="5 moles"`
`"Molality"=("0.0555 mol")/("0.090 kg")=0.617 m"`
`"x (Glucose)"=(0.0555)/(5+0.555)=0.01, x(H_(2)O)=1-0.01=0.99`
`"100 g solution"=(100)/(1.2)mL = "83.33 mL = 0.08333 K , Molarity "=("0.0555 mol")/("0.08333 L")="0.67 M".`