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,…
Solutions · Class 12 · JEE Main Previous Year 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.
- a✓
- b
- c
- d
Strategy:\n> 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 .\n\nStep 1: Compare concentrations\n- Solution A: 0.1 M (Highest concentration)\n- Solution B: 0.01 M\n- Solution C: 0.001 M (Most dilute)\n\nStep 2: Relate concentration to dissociation/ion-pairing\n- In Solution C (very dilute), is most "freely" dissociated. is closest to 2.\n- In Solution A (more concentrated), ion interactions are strongest. is lowest.\n\nConclusion:\nThe van't Hoff factor value follows the order: .\n\n
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