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Dissolving 120 g of a compound of (mol. wt. 60) in 1000 g of water gave a solution of density 1.12 g/mL. The molarity of the solution is:
  • a)
    1.00 M
  • b)
    2.00 M
  • c)
    2.50 M
  • d)
    4.00 M
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
Dissolving 120 g of a compound of (mol. wt. 60) in 1000 g of water ga...
To find the molarity of the solution, we need to first calculate the number of moles of the compound and the volume of the solution.

Given:
Mass of the compound = 120 g
Molar mass of the compound = 60 g/mol
Density of the solution = 1.12 g/mL
Volume of the solution = 1000 g

- Calculating the number of moles of the compound:

Number of moles = Mass of the compound / Molar mass
Number of moles = 120 g / 60 g/mol
Number of moles = 2 mol

- Calculating the volume of the solution:

Density = Mass / Volume
Volume = Mass / Density
Volume = 1000 g / 1.12 g/mL
Volume = 892.857 mL

- Converting the volume to liters:

Volume = 892.857 mL * (1 L / 1000 mL)
Volume = 0.892857 L

- Calculating the molarity:

Molarity = Number of moles / Volume
Molarity = 2 mol / 0.892857 L
Molarity ≈ 2.24 M

Since the molarity is approximately 2.24 M, the correct option is (B) 2.00 M.
Free Test
Community Answer
Dissolving 120 g of a compound of (mol. wt. 60) in 1000 g of water ga...
Given
mass of solute (w) = 120 g
mass of solvent (w) = 1000 g Mol.
mass of solute = 60 g
density of solution = 1.12 g/ mL
From the given data,
Mass of solution = 1000+ 120 = 1120 g
∴ d = Mol. mass / v or v = Mol. mass / d
Volume Solution
V = 1120/1.12 = = 1000 mL or = 1 litre
Now molarity (M ) = W / Mol. mass x V (lit.)
= 120/60 x 1
= 2M
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Dissolving 120 g of a compound of (mol. wt. 60) in 1000 g of water gave a solution of density 1.12 g/mL. The molarity of the solution is:a)1.00 Mb)2.00 Mc)2.50 Md)4.00 MCorrect answer is option 'B'. Can you explain this answer?
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