Compound PdCl₄.6H₂O is a hydrated complex, 1 molal aqueous solution of it has freezing point 269.28 K. Assuming 100 % ionization of complex, the molecular formula of the complex is-

(K_f for water = 1.86 K kg mole^-1)

1. [Pd(H₂O)₆]Cl₄

2. [Pd(H₂O)₄Cl₂]Cl₂.2H₂O

3. [Pd(H₂O)₃Cl₃]Cl.3H₂O

4. [Pd(H₂O)Cl₄]4H₂O

K₄[Fe(CN)₆] is 60% ionised. Then the value of Van't Hoff factor is

1. 1.6

2. 2.4

3. 3

4. 3.4

If molality of the dilute solution is doubled, the value of molal depression constant (K_f) will be?

(1) doubled

(2) halved

(3) tripled

(4) unchanged

The temperature dependent term among the following is -

The molar conductivity of a solution of AgNO₃ (considering the given data for this solution) at 298 K is:
(a) Concentration: 0.5 mol/dm³
(b) Electrolytic conductivity: 5.76×10^–3 S cm^–1

The van't Hoff factor [i] for a dilute aqueous solution of the strong electrolyte barium hydroxide is?

(1) 0

(2) 1

(3) 2

(4) 3

Which one of the following is incorrect for ideal solution ?

(1) $∆{\mathrm{H}}_{\mathrm{mix}}=0$

(2) $∆{\mathrm{U}}_{\mathrm{mix}}=0$

(3) $∆\mathrm{P}={\mathrm{P}}_{\mathrm{obs}}-{\mathrm{P}}_{\mathrm{calculated} \mathrm{by} \mathrm{Raoul}\text{'}\mathrm{s} \mathrm{law}} = 0$

(4) $∆{\mathrm{G}}_{\mathrm{mix}}=0$

At 100°C the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If K_b = 0.52, the boiling point of this solution will be

(1) 100°C

(2) 102°C

(3) 103°C

(4) 101°C

Which of the following statements about the composition of the vapour over an ideal 1:1

molar mixture of benzene and toluene is correct? Assume that the temperature is

constant at 25°C.

(Given, vapour pressure data at 25°C, benzene = 12.8 kPa, toluene = 3.85 kPa)

1. The vapour will contain a higher percentage of toluene

2. The vapour will contain equal amounts of benzene and toluene

3. Not enough information is given to make a prediction

4. The vapour will contain a higher percentage of benzene

Which one is not equal to zero for an ideal solution?

1. ΔH_mix 

2. ΔS_mix

3. ΔV_mix

4. ΔP=P_Observed-P_Raoult