A solution of glucose in water is labelled as `10 % 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 percent w/w solution of glucose I water means 10 g glucose and 90 g of water.
Molar mass of glucose`=180g" "mol^(-1)` and molar mass of water `=18" "mol^(-1)`.
`10g` of glucose `=(10)/(180=0.0555` moles
and 90g of `H_(2)O=(90)/(18)=5` moles
`therefore` molality of solution
`=("Moles of solute"xx1000)/("Mass of solution in grams")`
`=(0.555)/(90)xx1000=0*617`m
Mole fraction of glucose.
Mole fraction of glucose.
`=X_(g)=("No of moles of glucose")/("No. of moles+No. of moles of glucose of water")`
`=(0*0555)/(5+0*0555)=0.01`
mole fraction of water
`X_(w)=("No. of moles of water")/("No. of moles+No. of glucose moles of water")`
`=(5)/(5+0*0555)=0*99`
Volume of 100g of solution
`=("Mass of solution")/("Density")=(100)/(1*2)=83*33mL`
`therefore` Molarity of solution `=(0*0555)/(83*33)xx1000`
`=0*67M`.