Which of the following statements is correct | vedclass

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(B) Calculate the molarity $(M)$ of the urea solution: $M_{urea} = \frac{6 \ g \ L^{-1}}{60 \ g \ mol^{-1}} = 0.1 \ mol \ L^{-1}$.Calculate the molari

Vedclass · Accepted Answer

Urea solution is hypertonic to sucrose solution.

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(B) Calculate the molarity $(M)$ of the urea solution: $M_{urea} = \frac{6 \ g \ L^{-1}}{60 \ g \ mol^{-1}} = 0.1 \ mol \ L^{-1}$.Calculate the molarity $(M)$ of the sucrose solution: $M_{sucrose} = \frac{17.12 \ g \ L^{-1}}{342 \ g \ mol^{-1}} \approx 0.05 \ mol \ L^{-1}$.Since osmotic pressure $\pi = CRT$,and the temperature $(T)$ is constant,the solution with higher molar concentration has higher osmotic pressure.As $0.1 \ M > 0.05 \ M$,the urea solution has a higher osmotic pressure than the sucrose solution.Therefore,the urea solution is hypertonic to the sucrose solution.

Which of the following statements is correct for an aqueous solution of $6 \ g \ L^{-1}$ urea and $17.12 \ g \ L^{-1}$ sucrose? [Molar mass of urea $= 60 \ g \ mol^{-1}$,Molar mass of sucrose $= 342 \ g \ mol^{-1}$]

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