A solution containing 10 g/L of urea is isot | vedclass

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(D) For isotonic solutions,the molar concentrations are equal: $C_1 = C_2$.Concentration of urea $(C_1)$: Urea molar mass is $60 \ g/mol$.$C_1 = \frac

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$300$

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(D) For isotonic solutions,the molar concentrations are equal: $C_1 = C_2$.Concentration of urea $(C_1)$: Urea molar mass is $60 \ g/mol$.$C_1 = \frac{10 \ g/L}{60 \ g/mol} = \frac{10}{60} \ mol/L$.Concentration of non-electrolyte $(C_2)$: $A$ $5\%$ solution means $5 \ g$ of solute in $100 \ mL$ of solution.This equals $50 \ g$ of solute in $1000 \ mL$ $(1 \ L)$ of solution.$C_2 = \frac{50 \ g}{M \ g/mol} = \frac{50}{M} \ mol/L$,where $M$ is the molecular mass.Since the solutions are isotonic,$C_1 = C_2$:$\frac{10}{60} = \frac{50}{M}$$M = \frac{50 	imes 60}{10} = 300 \ g/mol$.

$A$ solution containing $10 \ g/L$ of urea is isotonic with a $5\%$ solution of a non-electrolyte solute. The molecular mass of the non-electrolyte solute is ..... $g/mol$.

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