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(B) The osmotic pressure $(\pi)$ of a solution is given by the van't Hoff equation: $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar c

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$\pi \propto 1/	ext{molecular mass}$

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(B) The osmotic pressure $(\pi)$ of a solution is given by the van't Hoff equation: $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.For a very dilute solution,the molar concentration $C$ is approximately equal to the molality $m$ because the density of the solution is approximately equal to the density of the solvent.However,looking at the relationship $\pi = iCRT$,$\pi$ is directly proportional to $C$ (molarity) and $T$ (temperature).If we consider the definition of molarity $C = n/V$,where $n$ is the number of moles $(n = 	ext{mass}/	ext{molecular mass})$,then $\pi = (i 	imes 	ext{mass} 	imes R 	imes T) / (	ext{molecular mass} 	imes V)$.Thus,for a fixed mass of solute and fixed volume,$\pi \propto 1/	ext{molecular mass}$.

For a very dilute solution of an electrolyte,which of the following relations is correct? (Assume other parameters are constant)

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