The boiling point of 0.2 mol kg^-1 solution of X in water is greater than equimolal solution

of Y in water. Which one of the following statements is true in this case?

1. X is undergoing dissociation in water

2. Molecular mass of X is greater than the molecular mass of Y

3. Molecular mass of X is less than the molecular mass of Y

4. Y is undergoing dissociation in water while X undergoes no change

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)? 

1. K₂SO₄

2. K₃[Fe(CN)₆]

3. Al(NO₃)₃

4. K₄[Fe(CN)₆]

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

point depression?

1. KCl

2. C₆H₁₂O₆

3. Al₂(SO₄)₃

4. K₂SO₄

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.

1. p_A + x_A(p_B-p_A)

2. p_A + x_A(p_A-p_B)

3. p_B + x_A(p_B-p_A)

4. p_B + x_A(p_A-p_B)

Limiting molar conductivity of NH₄OH (i.e Åm(NH₄OH)) is equal to:-

1. Å_m (NH₄Cl)+Å_m(NaCl)-Å_m(NaOH) 

2. Å_m(NaOH)+Å_m(NaCl)-Å_m(NH₄Cl)

3. Å_m(NH₄OH)+Å_m(NH₄Cl)-Å_m(HCl)

4. Å(NH₄Cl)+Å(NaOH)-Å(NaCl)

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

1. 2.63

2. 3.11

3. 0.381

4. 2.05

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

association in other solvent is respectively.

1. less than one and less than one

2. greater than one and less than one

3. greater than one and greater than one

4. less than one and greater than one

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

the solution to increase ?

1. Addition of NaCl

2. Addition of Na₂SO₄

3. Addition of 1.00 molal KI

4. Addition of water

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)

1. -0.372 $°$C

2. 0.372 $°$C

3. 0.572 $°$C

4. -0.572 $°$C

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due

to

1. increase in ionic mobility of ions

2. 100% ionisation of electrolyte at normal dilution

3. increase in both, i.e. number of ions and ionic mobility of ions

4. increase in number of ions