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?
Lost your password? Please enter your email address. You will receive a link and will create a new password via email.
Please briefly explain why you feel this question should be reported.
Please briefly explain why you feel this answer should be reported.
Please briefly explain why you feel this user should be reported.
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`.