Solutions and Colligative Properties

In a 0.2 molal aqueous solution of a weak acid HX the degree of ionization is 0.3. Taking k_f for water as 1.85, the freezing point of the solution will be nearest to

If liquids A and B form an ideal solution

Which one of the following statements is false?

Which one of the following aqueous solutions will exhibit highest boiling point?

If $\alpha$ is the degree of dissociation of Na₂SO₄, the vant Hoff’s factor (i) used for calculating the molecular mass is :

Among the following mixtures, dipole-dipole as the major interaction, is present in

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water (∆T_f), when 0.01 mol of sodium sulphate is dissolved in 1 kg of water, is (K_f = 1.86 K kg mol^–1)

The degree of dissociation ($\alpha$ ) of a weak electrolyte, A_xB_y is related to van’t Hoff factor (i) by the expression :

K_f for water is 1.86K kg mol^–1. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol (C₂H₆O₂) must you add to get the freezing point of the solution lowered to –2.8^oC ?

Consider separate solutions of 0.500 M C₂H₅OH(aq), 0.100 M Mg₃(PO₄)₂(aq), 0.250 M KBr(aq) and 0.125 M Na₃PO₄(aq) at 25^oC. Which statement is true about these solutions, assuming all salts to be strong electrolytes?

An aqueous solution of a salt MX₂ at certain temperature has a van’t Hoff factor of 2. The degree of dissociation for this solution of the salt is :

The freezing point of benzene decreases by 0.45⁰C when 0.2 g of acetic acid is added to 20g of benzene. If acetic acid associates to form a dimer in benzene, percentage association of acetic acid in benzene will be: (K_f for benzene = 5.12 K kg mol^–1)

5 g of Na₂SO₄ was dissolved in x g of H₂O. The change in freezing point was found to be 3.82^oC. If Na₂SO₄ is 81.5% ionised, the value of x (K_f for water=1.86^oC kg mol^−1) is approximately : (molar mass of S = 32 g mol^−1 and that of Na = 23 g mol^−1)

For 1 molal aqueous solution of the following compounds, which one will show the highest freezing point?

Molecules of benzoic acid (C₆H₅COOH) dimerise in benzene. 'w' g of the acid dissolved in 30 g of benzene shows a depression in freezing point equal to 2K. If the percentage association of the acid to form dimmer in the solution is 80, then w is – (Its given that K_f = 5 K kg mol^–1, Molar mass of benzoic acid = 122 g mol^–1)

Molal depression constant for a solvent is 4.0 kg mol^–1. The depression in the freezing point of the solvent for 0.03 mol kg^–1 solution of K₂SO₄ is : (Assume complete dissociation of the electrolyte)

K₂Hgl₄ is 40% ionised in aqueous solution. The value of its van't Hoff factor (i) is:

The freezing point of a diluted milk sample is found to be –0.2^oC, while it should have been –0.5^oC for pure milk. How much water has been added to pure milk to make the diluted sample?

Which one of the following 0.06 M aqueous solutions has lowest freezing point?