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Calculate the Molarity of a solution of ethanol in water in which the mole fraction of ethanol is 0.040 (assume the density of water to be one).
By BYJU'S Exam Prep
Updated on: September 25th, 2023
The molarity of a solution of ethanol in water in which the mole fraction of ethanol is 0.040 is 2.1M
Now we have to calculate the molarity
The number of moles of solute per litre of solution is known as the molarity (M) of a solution.
Molarity = no. of moles of solute/ litres of solution
Step 1: Now we have determine the number of moles of ethanol and water
Moles of Water = 1 – 0.04
Moles of Ethanol = 0.04 Mol
Moles of Water = 0.96Mol
Step 2: Now we have to determine the mass of ethanol and water
Number of moles = Given mass/ Molar mass
Mass = number of moles x molar mass
Mass of water = 0.96 x 18
Mass of water = 17.3 g
Mass of ethanol = 0.04 x 46
Mass of ethanol = 1.84 g
Step 3: Now we have to determine the total mass of soluion
Total mass of the solution = 17.3 + 1.84
Total mass of the solution = 19.1 g
Table of content
Step 4: Now we have to determine the volume
Density = 1g/mL (Assumed)
Density = mass/ volume
On rearranging we get
Volume = mass/ density
Volume = 19.1/1
Volume = 19.1 mL
Volume = 0.0191 L
Determination of Molarity
Molarity = 0.04/0.0191
Molarity = 2.1 M
Consequently, a solution of ethanol in water has a molarity of 2.1M.
Summary:-
Calculate the Molarity of a solution of ethanol in water in which the mole fraction of ethanol is 0.040 (assume the density of water to be one).
A solution of ethanol in water with a mole fraction of 0.040 has a molarity of 2.1M. Ethanol is a plant fermentation by-product which is natural and it can also be produced through the hydration of ethylene.
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