Chemistry - Liquid Solution Question with Solution | TestHub

Osmotic pressure is given by $\pi =iCRT$.

For non-electrolytes like urea and glucose, the van't Hoff factor $i=1$.

For two solutions to exhibit the same osmotic pressure at a given temperature, their molar concentrations must be equal ($C_1=C_2$).

Molar concentration $C=\frac{\text{mass per unit volume}}{\text{molar mass}}$.

For $6$ g/L urea solution:
$C_{\text{urea}}=\frac{6}{60}=0.1$ mol/L

For $18$ g/L glucose solution:
$C_{\text{glucose}}=\frac{18}{180}=0.1$ mol/L

Since $C_{\text{urea}}=C_{\text{glucose}}$, these two solutions are isotonic and exhibit the same osmotic pressure.

Answer: $6$ g/L urea solution and $18$ g/L glucose solution.