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(A) The van 't Hoff factor $(i)$ for a strong electrolyte like $NaCl$ increases as the concentration decreases.In more concentrated solutions (like $0

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$i_A < i_B < i_C$

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(A) The van 't Hoff factor $(i)$ for a strong electrolyte like $NaCl$ increases as the concentration decreases.In more concentrated solutions (like $0.1 \ M$),interionic attractions are stronger,which reduces the effective dissociation.As the solution becomes more dilute (from $A$ to $C$),the ions move further apart,and $i$ approaches its theoretical maximum value of $2$.Therefore,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 van 't Hoff factor $(i)$ for these solutions will be in the order:

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