List of top Chemistry Questions on Colligative Properties asked in UP Board XII

The aqueous solution having maximum boiling point is

Explain Raoult's Law. The vapour pressure of chloroform (\( \text{CHCl}_3 \)) and dichloromethane (\( \text{CH}_2\text{Cl}_2 \)) are 200 mm Hg and 4.5 mm Hg respectively at 298 K. Calculate the vapour pressure of the solution formed by mixing 51 g of \( \text{CHCl}_3 \) and 20 g of \( \text{CH}_2\text{Cl}_2 \) at 298 K.

Find the osmotic pressure of $\dfrac{M{10}$ urea solution at $27^\circ\mathrm{C}$ \ (Given: $R=0.0821$ L\,atm\,K$^{-1}$\,mol$^{-1}$).}

6 g urea is dissolved in 200 g water. Calculate the elevation in boiling point. Molal elevation constant for water is 0.52 K kg mol$^{-1$.}

Write the definition of osmotic pressure. Calculate the osmotic pressure of 2% aqueous solution of urea at 27$^\circ$C. Solution constant $R = 0.082\ \text{L atm K^{-1}\ \text{mol}^{-1}$.}

What is elevation of boiling point? A liquid has boiling point 353.23 K. The boiling point of solution becomes 354.11 K after dissolving 1.8 g non-volatile solute of molar mass 58 g mol$^{-1$ to 90 g liquid. Calculate boiling point elevation constant for the liquid.}

At what temperature does a 5% (w/v) solution of glucose produce 7 atmospheric osmotic pressure? \([ R = 0.0821 \, \text{L} \cdot \text{atm} / \text{K mol} ]\)

Which one between 0.1 M Urea and 0.1 M NaCl solution will have greater osmotic pressure? Explain the reason.

Explain Raoult's law for solutions containing non-volatile solute in volatile solvent. Derive mathematical expression for this law.

The colligative property of a solution depends upon

Define molal elevation constant. Calculate the boiling point of an aqueous solution containing 0.6 g of urea (molar mass = 60) in 100 g of water. The value of molal elevation constant for water is 0.52 K kg mol\(^{-1}\) and boiling point of water is 373.15 K.

What is the effect of catalyst on the rate of reaction? A first-order reaction is 40\% completed in 50 minutes. Calculate the time taken for 80\% completion of the reaction. (Given: \(\log 2 = 0.3010\) and \(\log 6 = 0.7782\))

Define molal depression constant. Calculate the freezing point of the aqueous solution containing 25 g of ethylene glycol (C\(_2\)H\(_6\)O\(_2\)) in 300 g of water. The value of molal depression constant for water is 1.86 K kg mol\(^{-1}\) and freezing point of water is 273.15 K.

2.82 g of glucose (molar mass = 180 g mol\(^{-1}\)) is dissolved in 30 g of water. Calculate the molality of the solution.

What is osmotic pressure? Explain the difference between osmosis and diffusion with an example.

The colligative property is