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(A) Osmotic pressure $\pi = CRT$, where $C$ is molarity. For the same temperature $T$, solutions with the same molarity $C$ have the same osmotic pres

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$6 	ext{ g/L}$ urea solution and $18 	ext{ g/L}$ glucose solution.

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(A) Osmotic pressure $\pi = CRT$, where $C$ is molarity. For the same temperature $T$, solutions with the same molarity $C$ have the same osmotic pressure.Step $1$: Calculate molarity $C = \frac{	ext{mass (g/L)}}{	ext{molar mass (g/mol)}}$.Step $2$: For urea $(M = 60 	ext{ g/mol})$, $C_1 = \frac{6 	ext{ g/L}}{60 	ext{ g/mol}} = 0.1 	ext{ M}$.Step $3$: For glucose $(M = 180 	ext{ g/mol})$, $C_2 = \frac{18 	ext{ g/L}}{180 	ext{ g/mol}} = 0.1 	ext{ M}$.Step $4$: Since $C_1 = C_2$, the osmotic pressures are equal.

Identify the pair of solutions that exhibits the same osmotic pressure. [Molar mass of urea $= 60 \text{ g mol}^{-1}$ and molar mass of glucose $= 180 \text{ g mol}^{-1}$]

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