MHT CET 2026 17th April Morning Shift | Liquid Solution Question 22 | Chemistry

Calculate van't Hoff factor for aqueous solution of 0.02 m formic acid if it freezes at -0.045 $^\circ\text{C}$.
[ $K_f$ = 1.86 K kg $\text{mol}^{-1}$ and freezing point of water = $0\ ^\circ\text{C}$ ]

$1.21$

$1.46$

$1.68$

$1.05$

MHT CET 2026 17th April Morning Shift

MCQ (Single Correct Answer)

-0

Calculate the molar mass of nonvolatile solute when 4 g of it is dissolved in 100 g solvent that boils at 319.4 K [$K_b$ = 2.4 K kg $\text{mol}^{-1}$; B.P of pure solvent = 319 K]

$220\ \text{gmol}^{-1}$

$230\ \text{gmol}^{-1}$

$240\ \text{gmol}^{-1}$

$250\ \text{gmol}^{-1}$

MHT CET 2026 16th April Evening Shift

MCQ (Single Correct Answer)

-0

The normal boiling point of Ethyl acetate is $77^\circ\text{C}$. A solution of non-volatile non-electrolyte solute in ethyl acetate boils at $78^\circ\text{C}$. $K_b$ for ethyl acetate is $2.77\ ^\circ\text{C kg mol}^{-1}$. What is the molality of the solution ?

$0.361\ \text{m}$

$0.052\ \text{m}$

$0.075\ \text{m}$

$0.25\ \text{m}$

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