At 0^{circ} C, a urea solution has an osmotic | vedclass

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(A) The osmotic pressure formula is $\pi = CRT$, where $C$ is the molar concentration $(n/V)$.For the initial state: $\pi_1 = C_1 RT_1$, where $\pi_1

Vedclass · Accepted Answer

$4.3$

Vedclass · Answer

(A) The osmotic pressure formula is $\pi = CRT$, where $C$ is the molar concentration $(n/V)$.For the initial state: $\pi_1 = C_1 RT_1$, where $\pi_1 = 400 \ mm$ and $T_1 = 273 \ K$.For the final state: $\pi_2 = C_2 RT_2$, where $\pi_2 = 100 \ mm$ and $T_2 = 293 \ K$.Taking the ratio: $\frac{\pi_1}{\pi_2} = \frac{C_1 T_1}{C_2 T_2}$.Since $C_1/C_2 = V_2/V_1 = x$, we have $\frac{400}{100} = x 	imes \frac{273}{293}$.Solving for $x$: $x = 4 	imes \frac{293}{273} \approx 4 	imes 1.073 = 4.292$.Thus, the dilution factor $x$ is approximately $4.3$.

At $0^{\circ} C$, a urea solution has an osmotic pressure of $400 \ mm$. On dilution by $x$ times, its osmotic pressure decreases to $100 \ mm$ at $20^{\circ} C$. The dilution factor $x$ is approximately

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