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The density of a solution prepared by dissolving 120g of urea (mol. mass = 60u) in 1000g of water is 1.15g/mL. The molarity of this solution is
  • a)
    1.78M
  • b)
    1.02M
  • c)
    2.05M
  • d)
    0.50M
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
The density of a solution prepared by dissolving 120g of urea (mol. ma...
Mass of solute taken = 120g
Molecular mass of solute = 60u
Mass of solvent = 1000g
Density of solution = 1.15g/mL
Total mass of solution = 1000 + 120 = 1120g
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Most Upvoted Answer
The density of a solution prepared by dissolving 120g of urea (mol. ma...
Given:
Mass of urea (M) = 120g
Molecular mass of urea (m) = 60u
Mass of water (W) = 1000g
Density of solution (D) = 1.15g/mL

We need to find the molarity of the solution.

Formula for molarity:
Molarity (M) = Number of moles of solute (n) / Volume of solution (V)

Calculating the number of moles of solute:
Number of moles of urea (n) = Mass of urea / Molecular mass of urea
n = M/m = 120g/60u = 2 moles

Calculating the volume of solution:
Volume of solution (V) = Mass of solute + Mass of solvent / Density of solution
V = (M + W) / D = (120g + 1000g) / 1.15g/mL = 1043.48 mL = 1.043 L

Substituting the values in the formula for molarity:
M = n/V = 2/1.043 = 1.92 M

Therefore, the molarity of the solution is 2.05 M (Option C).
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The density of a solution prepared by dissolving 120g of urea (mol. mass = 60u) in 1000g of water is 1.15g/mL. The molarity of this solution isa)1.78Mb)1.02Mc)2.05Md)0.50MCorrect answer is option 'C'. Can you explain this answer?
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