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(A) For isotonic solutions,the osmotic pressure $(\pi)$ is equal,which implies that their molar concentrations $(C)$ are equal at the same temperature

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$210$

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(A) For isotonic solutions,the osmotic pressure $(\pi)$ is equal,which implies that their molar concentrations $(C)$ are equal at the same temperature.Given that the solutions are $5.25\%$ and $1.5\%$ by mass,and assuming the density is $1.0\ g\ cm^{-3}$,the concentration in $g\ L^{-1}$ is the same as the percentage mass multiplied by $10$.Concentration of substance $(C_1) = \frac{5.25 	imes 10}{M} = \frac{52.5}{M} \ mol\ L^{-1}$.Concentration of urea $(C_2) = \frac{1.5 	imes 10}{60} = \frac{15}{60} = 0.25 \ mol\ L^{-1}$.Since the solutions are isotonic,$C_1 = C_2$.$\frac{52.5}{M} = 0.25$.$M = \frac{52.5}{0.25} = 210 \ g\ mol^{-1}$.

$A$ $5.25\%$ solution of a substance is isotonic with a $1.5\%$ solution of urea (molar mass $= 60\ g\ mol^{-1}$) in the same solvent. If the densities of both the solutions are assumed to be equal to $1.0\ g\ cm^{-3},$ the molar mass of the substance will be .............. $g\ mol^{-1}$.

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