When 0.1 m CH₃COOH is present in a solvent it shows elevation in boiling point of 0.75$°\mathrm{C}$. Acid dissociation constant will be -(K_b=5 K Kg mol^-1) (1M =1m)

Which of the following shows positive deviation from Raoult's law:

(i) Chloroform and acetone

(ii) Carbon disulphide and acetone

(iii) Ethanol and Acetone

(iv) Phenol and Aniline

A non-volatile solute is dissolved in water. If its degree of association is 50%. What will be its freezing point when the boiling point is 100.52$°\mathrm{C}$. [K_b=0.52 K kg mol^-1, K_f=1.86K kg mol^-1]

When 36 g of a solute having the emperical formula CH₂O is dissolved in 1.2 kg of water, the solution freezes at -0.93$°\mathrm{C}$. What is the molecular formula of solute (K_f=1.86 kg K mol^-1)

If partial pressure of oxygen is 0.5 atm and K_H=1.4 X 10^-3 M/atm. The amount of oxygen is dissolved in 100ml water at 298K is-

A solute x when dissolved in solvent associates to form a pentamer. The value of van't hoff factor (i) for the solute will be:-

What amount of CaCl₂(i=2.47) is dissolved in 2L water so that its osmotic pressure is 0.5 atm at 27$°\mathrm{C}$:-

One litre aqueous solution of sucrose (molar mass = 342 g/mol) weighing 1015 g is found to record an osmotic pressure of 4.8 atm at 293K. What is the molality of the sucrose solution ? (R= 0.0821 L atm K^-1 mol^-1) :

The total vapor of a solution of liquid A and liquid B is 600 torr. The mole fraction of component A in the liquid phase is 0.7 and in the vapor phase is 0.35. The vapor pressure of pure A and B are respectively

The vapour pressure of water at room temperature is 30 mm of Hg. If the mole fraction of the water is 0.9, the vapour pressure of solution will be

The Van't Hoff factor of a 0.005 M aqueous solution of KCl is 1.95. The degree of ionisation of KCl is-

The solution having highest vapour pressure is (Assume 100% ionisation of electrolytes)

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

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

(K_f for water = 1.86 K kg mole^-1)

In a cold climate frozen causing damage to radiator of a car. Ethylene glycol is used as antifreezing agent. The amount of ethylene glycol to be added to 4 kg of water to prevent it from freezing at $-6°C$. $[k_f for water=1.85 k kg mo{l}^{-1}]$

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

Temperature dependent term among the following is -

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

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)

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

Which one of the following elctrolytes has the same value of van't Hoff's factor(i) as

that of Al₂(SO₄)₃  (if all are 100% ionised)? 

Of the following 0.10 m  aqueous solutions, which one will exhibit the largest freezing

point depression?

p_A and p_B are the vapour pressure of pure liquid components, A and B, respectively of an

ideal binary solution.If x, represents the mole fraction of component A, the total pressure

of the solution will be.

The freezing point depression constant format is -1.86°C m^-1. If 5.00g Na₂SO₄ dissolved

in 45.0 g H₂O, the freezing point is changed by -3.82°C. Calculate the van't Hoff factor

for NaSO4

The van't Hoff factor, i for a compound which undergoes dissociation in one solvent and

association in other solvent is respectively.

An aqueous solution is 1.00 molal in KI. Which change will cause the vapour pressure of

the solution to increase ?

A solution of sucrose (molar mass = 342 g mol^-1) has been prepared by dissolving 68.5 g

of sucrose in 1000 g of water. The freezing point of the solution obtained will be (K_f for

water = 1.86 K kg mol^-1)-

A 0.0020 m aqueous solution of an ionic compound Co(NH₃)₅(NO₂)Cl freezes at -0.00732°C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (k_f=-1.86^$°$C/ m)

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_f for water is 1.86 K kg mol^-1, the lowering in freezing point of the solution is:

1.00 g of a non-electrolyte solute (molar mass 250g/mol) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K_f of benzene is 5.12 K kg mol^-1, the freezing point of benzene will be lowered by:-