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(B) Two solutions are isotonic if they have the same osmotic pressure $(\pi)$. For a solution,$\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is m

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$A$ and $C$

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(B) Two solutions are isotonic if they have the same osmotic pressure $(\pi)$. For a solution,$\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is molarity,$R$ is the gas constant,and $T$ is temperature.For non-electrolytes like glucose and urea,$i = 1$. For electrolytes,$i$ is the number of ions produced.$(A)$ Glucose $(18 \ g/L)$: $C = 18/180 = 0.1 \ M$. Urea $(6 \ g/L)$: $C = 6/60 = 0.1 \ M$. Since $C_1 = C_2$,$\pi_1 = \pi_2$. Thus,$A$ is isotonic.$(B)$ Glucose $(10 \ g/L)$: $C = 10/180 \approx 0.056 \ M$. Urea $(10 \ g/L)$: $C = 10/60 \approx 0.167 \ M$. $\pi_1 
eq \pi_2$.$(C)$ $NaOH$ $(0.01 \ M)$: $i = 2$ $(Na^+ + OH^-)$,so $\pi = 2 	imes 0.01 	imes RT = 0.02 \ RT$. Glucose $(0.02 \ M)$: $i = 1$,so $\pi = 1 	imes 0.02 	imes RT = 0.02 \ RT$. Since $\pi_1 = \pi_2$,$C$ is isotonic.$(D)$ $NaCl$ $(0.01 \ M)$: $i = 2$,so $\pi = 2 	imes 0.01 	imes RT = 0.02 \ RT$. Glucose $(0.01 \ M)$: $i = 1$,so $\pi = 0.01 	imes RT$. $\pi_1 
eq \pi_2$.Therefore,both $A$ and $C$ are isotonic pairs.

List-$I$	List-$II$
$A$. van't Hoff factor,$i$	$I$. Cryoscopic constant
$B$. $k_{f}$	$II$. Isotonic solutions
$C$. Solutions with same osmotic pressure	$III$. $\frac{\text{Normal molar mass}}{\text{Abnormal molar mass}}$
$D$. Azeotropes	$IV$. Solutions with same composition of vapour above it

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