A solution containing 6.0 g of urea is isoto | vedclass

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(B) Two solutions having the same osmotic pressure at a given temperature are called isotonic solutions. For isotonic solutions,the molar concentratio

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$100$

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(B) Two solutions having the same osmotic pressure at a given temperature are called isotonic solutions. For isotonic solutions,the molar concentrations are equal: $C_{urea} = C_{X}$. The formula for molar concentration is $C = \frac{W}{M 	imes V(L)}$. Since the volumes are the same,we have $\frac{W_{urea}}{M_{urea}} = \frac{W_{X}}{M_{X}}$. The molar mass of urea $(NH_2CONH_2)$ is $60 \ g \ mol^{-1}$. Substituting the given values: $\frac{6.0}{60} = \frac{10}{M_{X}}$. $0.1 = \frac{10}{M_{X}}$. $M_{X} = \frac{10}{0.1} = 100 \ g \ mol^{-1}$. Thus,the molar mass of $X$ is $100 \ g \ mol^{-1}$.

$A$ solution containing $6.0 \ g$ of urea is isotonic with a solution containing $10 \ g$ of a non-electrolytic solute $X$. The molar mass of $X$ (in $g \ mol^{-1}$) is

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