Question

a solution is 10% aqueous solution of glucose having density 1.02 gram per CC find out its molarity molality and mole fraction​

Answer 1

mass of C6H12O6 =10g

mass of solution =100g

mass of H2O = 90 g

density = 1.02

density = mass of solution/ volume

1.02 = 100/ volume

volume = 100/ 1.02

molar mass of C6H12O6= 180

molar mass of H20 =18

moles of glucose = 10/180

=0.06

moles of H2O = 90/ 18

= 5

molarity = moles of glucose ×1000/ volume of solution

= 0.06×1000/[100/1.02]

M = 0.612 M/mol

molality= moles of glucose ×1000/ mass of solvent

= 0.06 ×1000/90

= 60/ 90

= 2/3

m =0.67 m /mol

mole fraction X [ glucose] = moles [glucose]/ moles[ glucose] + moles [Water]

= 0.06/ 0.06+ 5

= 0.06/ 5.06

= 0.012

mole fraction [ water] + mole fraction [ glucose] =1

mole fraction [water] = 1- 0.012

= 0.988

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