Solutions — JEE Advanced PYQs

In a solvent S, a compound B is partially dissociated into C and D as given below:

B, C and D are non-volatile in nature. The molar mass of B is 10 times the molar mass of S. The standard boiling point and the standard e …

Two volatile liquids A and B form an ideal solution. Consider a 5 molal solution of B in A inside a closed container having a total vapour pressure of 100 mm Hg at 300 K. The vapour pressure of pure A at 300 K is 105 mm Hg. Assume that $\mathbf{A}$ and $\mathbf{B}$ behave as idea …

Two volatile liquids A and B form an ideal solution. Consider a 5 molal solution of B in A inside a closed container having a total vapour pressure of 100 mm Hg at 300 K. The vapour pressure of pure A at 300 K is 105 mm Hg. Assume that $\mathbf{A}$ and $\mathbf{B}$ behave as idea …

At 300 K, an ideal dilute solution of a macromolecule exerts osmotic pressure that is expressed in terms of the height (h) of the solution (density $=1.00\mathrm{g}{\mathrm{cm}}^{-3}$) where h is equal to 2.00 cm. If the concentration of the dilute solution of the macromolecule …

Vessel-1 contains ${\mathbf{w}}_2\mathbf{g}$ of a non-volatile solute $\mathbf{X}$ dissolved in ${\mathbf{w}}_{1}g$ of water. Vessel-2 contains ${\mathbf{w}}_{2}g$ of another non-volatile solute $\mathbf{Y}$ dissolved in …

50 mL of 0.2 molal urea solution (density $=1.012\mathrm{g}{\mathrm{mL}}^{-1}$ at 300 K ) is mixed with 250 mL of a solution containing 0.06 g of urea. Both the solutions were prepared in the same solvent. The osmotic pressure (in Torr) of the resulting solution at 300 K is _ …

An aqueous solution is prepared by dissolving 0.1 mol of an ionic salt in 1.8 kg of water at 35 °C. The salt remains 90% dissociated in the solution. The vapour pressure of the solution is 59.724 mm of Hg. Vapor pressure of water at 35 °C is 60.000 mm of Hg. The number of ions pr …

The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is ${\mathbf{x}}^{\circ }\mathrm{C}$. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in …

The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is ${\mathbf{x}}^{\circ }\mathrm{C}$. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in …

Liquids A and B form ideal solution for all compositions of A and B at 25°C. Two such solutions with 0.25 and 0.50 mole fractions of A have the total vapor pressures of 0.3 and 0.4 bar, respectively. What is the vapor pressure of pure liquid B in bar?

On dissolving 0.5 g of a non-volatile non-ionic solute to 39 g of benzene, its vapor pressure decreases from 650 mm Hg to 640 mm Hg . The depression of freezing point of benzene (in K) upon addition of the solute is ____
(Given data : Molar mass and the molal freezing point depre …

Liquids A and B form ideal solution over the entire range of composition. At temperature T, equimolar binary solution of liquids A and B has vapour pressure 45 Torr. At the same temperature, a new solution of A and B having mole fractions $x_A$ and $x_B$, respectively, ha …

The plot given below shows $P-T$ curves (where $P$ is the pressure and $T$ is the temperature) for two solvents $\mathbf{X}$ and $\mathbf{Y}$ and isomolal solutions of NaCl in these solvents. NaCl completely dissociates in both the solvents.

On addition of equal number …

Pure water freezes at 273 K and 1 bar. The addition of 34.5 g of ethanol to 500 g of water changes the freezing point of the solution. Use the freezing point depression constant of water as $2\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}$. The figures shown below represent plots o …

For a solution formed by mixing liquids L and M, the vapour pressure of L plotted against the mole fraction of M in solution is shown in the following figure. Here $x_L$ and $x_M$ represent mole fractions of L and M, respectively, in the solution. The corr …

The mole fraction of a solute in a solution is 0.1. At 298 K, molarity of this solution is the same as its molality. Density of this solution at 298 K is $2.0{\mathrm{g}\mathrm{cm}}^{-3}$. The ratio of the molecular weights of the solute and solvent, …

Mixture(s) showing positive deviation from Raoult's law at 35 °C is(are)

If the freezing point of a 0.01 molal aqueous solution of a cobalt(III) chloride-ammonia complex (which behaves as a strong electrolyte) is -0.0558 °C, the number of chloride(s) in the coordination sphere of the complex is
$[{\mathrm{K}}_{\mathrm{f}}$ of water …

${\mathbf{MX}}_2$ dissociates into ${\mathbf{M}}^{2+}$ and ${\mathbf{X}}^{-}$ 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 …

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 solu …

The freezing point (in °C) of a solution containing 0.1 g of ${\mathrm{K}}_3\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]$ (Mol. Wt. 329) in 100 g of water $({\mathrm{K}}_{\mathrm{f}}=1.86\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1})$ is

The Henry's law constant for the solubility of ${\mathrm{N}}_2$ gas in water at 298 K is $1.0\times 10^5\mathrm{atm}$. The mole fraction of ${\mathrm{N}}_2$ in air is 0.8. The number of moles of ${\mathrm{N}}_2$ from air dissolved in 10 moles of water at 298 K and 5 atm press …

Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of it …

Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of it …

Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of it …

75.2 g of ${\mathrm{C}}_6{\mathrm{H}}_5\mathrm{OH}$ (phenol) is dissolved in a solvent of ${\mathrm{K}}_{\mathrm{f}}=14$. If the depression in freezing point is 7 K then find the % of phenol that dimerises.