If 120 , g of urea (molar mass = 60 , g/mol) | vedclass

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Question

(C) Mass of solute (urea) = $120 \, g$ Molar mass of urea = $60 \, g/mol$ Moles of urea = $\frac{120}{60} = 2 \, mol$ Mass of solvent (water) = $1000

Vedclass · Accepted Answer

$2.05$

Vedclass · Answer

(C) Mass of solute (urea) = $120 \, g$ Molar mass of urea = $60 \, g/mol$ Moles of urea = $\frac{120}{60} = 2 \, mol$ Mass of solvent (water) = $1000 \, g$ Total mass of solution = $120 \, g + 1000 \, g = 1120 \, g$ Density of solution = $1.15 \, g/mL$ Volume of solution = $\frac{	ext{Mass}}{	ext{Density}} = \frac{1120}{1.15} \, mL = \frac{1120}{1.15 	imes 1000} \, L = \frac{1.12}{1.15} \, L$ Molarity $(M)$ = $\frac{	ext{Moles of solute}}{	ext{Volume of solution in } L} = \frac{2}{1.12 / 1.15} = \frac{2 	imes 1.15}{1.12} \approx 2.05 \, M$

If $120 \, g$ of urea (molar mass = $60 \, g/mol$) is dissolved in $1000 \, g$ of water and the density of the resulting solution is $1.15 \, g/mL$,what is the molarity of the solution in $M$?

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