The incorrect statement among the following for an ideal solution is:

1. \(\Delta H_{\text{Mix}}=0\)
2. \(\Delta U_{\text{Mix}}=0\)
3. \(\Delta P=P_{\text{obs.}}-P_{\text{(Calculated by Raoult's law)}}=0\)
4. \(\Delta G_{\text{Mix}}=0\)

Consider the following statements about the composition of the vapour over an ideal 1:1 molar mixture of benzene and toluene. The correct statement is:

Assume that the temperature is constant at 25 ^oC.
(Given, vapour pressure data at 25 °C, benzene = 12.8 kPa, toluene = 3.85 kPa)

The boiling point of 0.2 mol kg^–1 solution of X in water is greater than the equimolal solution of Y in water. The correct statement in this case is:

The electrolyte having the same value of Van't Hoff factor (i) as that of Al₂(SO₄)₃  (if all are 100% ionized) is:

The largest freezing point depression among the following 0.10 m solutions is shown by:

The freezing point depression constant for water is 1.86 ^oC m^-1. If 5.00 g Na₂SO₄ is dissolved in 45.0 g H₂O, the freezing point is changed by -3.82 ^oC. The Van’t Hoff factor for Na₂SO₄ is:

The van’t Hoff factor, i, for a compound that undergoes
dissociation and association in a 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. The vapour pressure of the solution can be increased by:

1. Addition of NaCl

2. Addition of Na₂SO₄

3. Addition of 1.00 molal Kl

4. Addition of water