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Consider the following aqueous solutions. I. 2.2 g Glucose in 125 mL of solution. II. 1.9 g Calcium chloride in 250 mL of solution. III. 9.0 g Urea in 500 mL of solution. IV. 20.5 g Aluminium sulphate in 750 mL of solution. The correct increasing order of boiling point of these solutions will be: [Given: Molar mass in g mol−1 - H = 1, C = 12, N = 14, O = 16, Cl = 35.5, Ca = 40, Al = 27 and S = 32]

1. I < II < III < IV
2. III < I < II < IV
3. III < II < I < IV
4. II < III < IV < I

Correct answer: I < II < III < IV

Solution

The boiling point elevation of a solution depends on the number of solute particles in the solution. Glucose (I) is a non-electrolyte and contributes fewer particles, while calcium chloride (II), urea (III), and aluminum sulfate (IV) dissociate into multiple ions, increasing the boiling point more significantly. Thus, the correct order reflects the increasing number of solute particles, leading to higher boiling points for solutions with more dissociated ions.

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