Colligative properties i.e., the properties of solution which depend upon the number of particle...

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Colligative properties i.e., the properties of solution which depend upon the number of particles present in
\( \mathrm{P} \) solution are osmotic pressure, depression in freezing

W point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electrolytes are always higher than those obtained theoretically because electrolytes dissociate to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute are lower than those obtained theoretically. The ratio of experimental colligative properties to theoretical colligative properties is called as vant Hoff factor \( (i) \).
A weak monoprotic acid (molar mass 180) aqueous solution of \( 0.18 \% \mathrm{w} / \mathrm{v} \) at \( 300 \mathrm{~K} \) has observed osmotic pressure \( 0.369 \mathrm{~atm} \). What should be its Vant Hoff factor (i). \( (\mathrm{R}=0.082 \mathrm{~atm} \times \mathrm{L} / \mathrm{K} \times \) mole \( ) \)
(A) \( 1.2 \)
(B) \( 1.5 \)
(C) 1
(D) \( 0.5 \)
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