MHT CET · Chemistry · Solutions
If \(0.01 \mathrm{~m}\) aqueous solution of an electrolyte freezes at \(-0.056{ }^{\circ} \mathrm{C}\). Calculate van't Hoff factor for an electrolyte. (Cryoscopic constant of water \(=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\) )
- A 1.3
- B 2.33
- C 3
- D 4.11
Answer & Solution
Correct Answer
(C) 3
Step-by-step Solution
Detailed explanation
\(\Delta \mathrm{T}_{\mathrm{f}}=\mathrm{i} \times \mathrm{K}_{\mathrm{f}} \times \mathrm{m}\)
\(0.056=\mathrm{i} \times 1.86 \times 0.01\)
\(\therefore \quad \mathrm{i}=\frac{0.056}{1.86 \times 0.01}=3.01\)
[Note: In the question, the freezing point of aqueous solution is changed from \(-0.056 \mathrm{~K}\) to \(-0.056^{\circ} \mathrm{C}\) to apply appropriate textual concepts.]
\(0.056=\mathrm{i} \times 1.86 \times 0.01\)
\(\therefore \quad \mathrm{i}=\frac{0.056}{1.86 \times 0.01}=3.01\)
[Note: In the question, the freezing point of aqueous solution is changed from \(-0.056 \mathrm{~K}\) to \(-0.056^{\circ} \mathrm{C}\) to apply appropriate textual concepts.]
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