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 for these solutions will be in the orde

Question

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 for these solutions will be in the order.

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Strategy:
 The van't Hoff factor () for a strong electrolyte like  is theoretically constant (). However, as concentration increases, interionic attractions and ion-pair formation increase, which effectively reduces the number of free particles and thus decreases the actual measured .

Step 1: Compare concentrations
- Solution A: 0.1 M (Highest concentration)
- Solution B: 0.01 M
- Solution C: 0.001 M (Most dilute)

Step 2: Relate concentration to dissociation/ion-pairing
- In Solution C (very d

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