The mole fraction of a solute in a solution is 0.1 At 298 K, Molarity of this solution is the same as its molality Density of this solution at 298 k is 2.0 g cm3. The ratio of the molecular weights of the solute and solvent,MW solute MW solvent , is?

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molecular weight of solute be =M1​and molecular weight of solvent be M2​fraction of solute =0.1Let solution be litremass of solution 1 litremass of solution =2000 gmass of solute =x man of solvent =2000−x.gMolarity=M1​x​/1litre=M1​x​Molarity=M1​x​/(2000−x)×10−3                  =(2000−x)M1​1000 x​                  Molarity=MolarityM1​x​=(2000−x)M1​1000 x​2000−x=1000x=1000 gMnumber of mole of solute =M1​1000​number of mole of solvent =M2​1000​M1​1000​+M2​1000​M1​1000​​⇒M1​+M2​M2​​=0.1M2​=0.1M1​+0.1M2​0.9M2​=0.1M1​⇒M2​M1​​=9

Question Text	The mole fraction of a solute in a solution is 0.1 At 298 K, Molarity of this solution is the same as its molality Density of this solution at 298 k is 2.0 g $c m^{3}$ . The ratio of the molecular weights of the solute and solvent,MW solute MW solvent , is?
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The mole fraction of a solute in a solution is 0.1 At 298 K, Molarity of this solution is the same as its molality Density of this solution at 298 k is 2.0 g $c m^{3}$ . The ratio of the molecular weights of the solute and solvent,MW solute MW solvent , is?

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