Solutions

A solution at 20°C is composed of 1.5 mol of benzene and 3.5 mol of toluene. If the vapour pressure of pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr, respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively :

Determination of the molar mass of acetic acid in benzene using freezing point depression is affected by :

$\ce{MX2}$ dissociates into $\ce{M^{2+}}$ and $\ce{X-}$ ions in an aqueous solution, with a degree of dissociation ($\alpha$) of 0.5. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is

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

Choose the correct statement with respect to the vapour pressure of a liquid among the following :

The observed osmotic pressure for a 0.10 M solution of $\ce{Fe(NH4)2(SO4)2}$ at 25°C is 10.8 atm. The expected and experimental (observed) values of Van't Hoff factor (i) will be respectively :

(R = 0.082 L atm k$^{-1}$ mol$^{-1}$)

For an ideal solution of two components A and B, which of the following is true ?

Benzene and naphthalene form an ideal solution at room temperature. For this process, the true statement(s) is(are)

For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in 100 g of water, the elevation in boiling point at 1 atm pressure is 2 °C. Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is (take $K_b=0.76$ K kg mol⁻¹)

To an evacuated vessel with movable piston under external pressure of 1 atm., 0.1 mol of He and 1.0 mol of an unknown compound (vapour pressure 0.68 atm. at 0 °C) are introduced. Considering the ideal gas behaviour, the total volume (in litre) of the gases at 0 °C is close to

The freezing point (in °C) of a solution containing 0.1 g of $\ce{K3[Fe(CN)6]}$ (Mol. Wt. 329) in 100 g of water ($K_f=1.86$ K kg mol$^{-1}$) is

The Henry's law constant for the solubility of $\ce{N2}$ gas in water at 298 K is $1.0\times10^5$ atm. The mole fraction of $\ce{N2}$ in air is 0.8. The number of moles of $\ce{N2}$ from air dissolved in 10 moles of water at 298 K and 5 atm pressure is

The freezing point of the solution M is

The vapour pressure of the solution M is

Water is added to the solution M such that the mole fraction of water in the solution becomes 0.9. The boiling point of this solution is

When 20 g of naphthoic acid ($\ce{C11H8O2}$) is dissolved in 50 g of benzene ($K_f=1.72$ K kg mol⁻¹), a freezing point depression of 2 K is observed. The van't Hoff factor ($i$) is