Solution A contains 7 g/L of MgCl_2 and solu | vedclass

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(B) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas

Vedclass · Accepted Answer

Osmotic pressure of $B$ is greater than $A$

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(B) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.For $MgCl_2$: $i = 3$ $(MgCl_2 ightarrow Mg^{2+} + 2Cl^-)$. Molar mass $M = 24 + 2 	imes 35.5 = 95 \ g/mol$. Concentration $C_A = 7 / 95 \ mol/L$.$\pi_A = 3 	imes (7/95) 	imes RT = (21/95)RT \approx 0.221RT$.For $NaCl$: $i = 2$ $(NaCl ightarrow Na^+ + Cl^-)$. Molar mass $M = 23 + 35.5 = 58.5 \ g/mol$. Concentration $C_B = 7 / 58.5 \ mol/L$.$\pi_B = 2 	imes (7/58.5) 	imes RT = (14/58.5)RT \approx 0.239RT$.Comparing the values,$\pi_B > \pi_A$.

Solution $A$ contains $7 \ g/L$ of $MgCl_2$ and solution $B$ contains $7 \ g/L$ of $NaCl$. Which of the following is true regarding their osmotic pressure at room temperature?

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