The density of a solution prepared by dissolving 120 g urea (mol. mass = 60 g/mol) in 1000 g of water is 1.15 g/ml. What is the molarity of the solution?

2.05 M

Mass of solution = 1000 + 120 = 1120 g

Volume of solution = \(\frac{mass}{density}\) = \(\frac{1120}{1.15}\)ml

Moles of urea = \(\frac{120}{60}\) = 2

Molarity = \(\frac{\text{Moles of urea}}{Volume}\)x1000

             = \(\frac{2}{1120/1.15}\) x 1000 = 2.05 M