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mole fraction=0.04
So if one mol of solution contain 0.04 mol of ethanol and (1-0.04)mol of water=0.96
So the mass of water=0.96*18 g=17.28g
So the mass of ethanol=0.04*46 g=1.84g
total mass=18.92g
Assuming the density of solution to be 1g/ml, the volume of the solution=18.92ml
So if 18.92ml of solution contain 0.04 mol of ethanol.
So …....1ml...............................0.04/18.92mol....
so 1000ml...............................(0.04/18.92)*1000=molarity of the solution=2.11M
So if one mol of solution contain 0.04 mol of ethanol and (1-0.04)mol of water=0.96
So the mass of water=0.96*18 g=17.28g
So the mass of ethanol=0.04*46 g=1.84g
total mass=18.92g
Assuming the density of solution to be 1g/ml, the volume of the solution=18.92ml
So if 18.92ml of solution contain 0.04 mol of ethanol.
So …....1ml...............................0.04/18.92mol....
so 1000ml...............................(0.04/18.92)*1000=molarity of the solution=2.11M
Answered by
5
mole fraction=0.04
So if one mole of solution contain 0.04 mole of ethanol and (1-0.04)mole of water=0.96
So the mass of water=0.96*18 g=17.28g
So the mass of ethanol=0.04*46 g=1.84g
total mass=18.92g
Assuming the density of solution to be 1g/ml, the volume of the solution=18.92ml
So if 18.92ml of solution contain 0.04 mol of ethanol.
So …....1ml...............................0.04/18.92mol....
so 1000ml...............................(0.04/18.92)*1000=molaritty of the solution=2.1M
So if one mole of solution contain 0.04 mole of ethanol and (1-0.04)mole of water=0.96
So the mass of water=0.96*18 g=17.28g
So the mass of ethanol=0.04*46 g=1.84g
total mass=18.92g
Assuming the density of solution to be 1g/ml, the volume of the solution=18.92ml
So if 18.92ml of solution contain 0.04 mol of ethanol.
So …....1ml...............................0.04/18.92mol....
so 1000ml...............................(0.04/18.92)*1000=molaritty of the solution=2.1M
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