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(C) The Van't Hoff factor $(i)$ for a strong electrolyte like $NaCl$ is given by the formula $i = 1 + (n-1)\alpha$,where $n$ is the number of ions pro

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$i_{A} < i_{B} < i_{C}$

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(C) The Van't Hoff factor $(i)$ for a strong electrolyte like $NaCl$ is given by the formula $i = 1 + (n-1)\alpha$,where $n$ is the number of ions produced per formula unit and $\alpha$ is the degree of dissociation.For $NaCl$,$n = 2$. As the concentration of the solution decreases,the degree of dissociation $(\alpha)$ increases due to the decrease in inter-ionic attractions.Therefore,as concentration decreases from $0.1 \ M$ to $0.001 \ M$,$\alpha$ increases,which leads to an increase in the value of $i$.Thus,the order of the Van't Hoff factor is $i_{A} < i_{B} < i_{C}$.

We have three aqueous solutions of $NaCl$ labelled as '$A$','$B$' and '$C$' with concentrations $0.1 \ M$,$0.01 \ M$,and $0.001 \ M$ respectively. The value of the Van't Hoff factor for these solutions will be in the order . . . . . . .

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