Solutions — JEE Main PYQs

1 g of non-volatile non-electrolyte solute is dissolved in 100 g of two different solvents A and B whose ebullioscopic constants are in the ratio of $1:5$. The ratio of the elevation in their boiling points, $\frac{\Delta T_b(A)}{\Delta T_b(B)}$ is :

The freezing point of diluted milk sample is found to be $-0.2^0\mathrm{C}$, while it should have been $-0.5^{\circ }\mathrm{C}$ for pure milk. How much water been added to pure milk to make the diluted sample?

Which of the following has lowest freezing point?

Freezing point of a 4% aqueous solution of X is equal to freezing point of 12% aqueous solution of Y. If molecular weight of X is A then molecular weight of Y is

A solution is prepared by dissolving 0.6 g of urea (molar mass $=60{\text{ g mol}}^{-1}$) and 1.8 g of glucose (molar mass $=180{\text{ g mol}}^{-1}$) in 100 mL of water at $27^{\circ }\text{C}$. The osmotic pressure of the solution is :
( …

Molecules of benzoic acid $({\mathrm{C}}_6{\mathrm{H}}_5\mathrm{COOH})$ dimerise in benzene. 'w' g of the acid dissolved in 30 g of benzene shows a depression in freezing point equal to 2 K. If the percentage association of the acid to form dimer in the solution is 80, then w i …

Molal depression constant for a solvent is $4.0\mathrm{K}\mathrm{Kg}{\mathrm{mol}}^{-1}$. The depression in the freezing point of the solvent for $0.03\mathrm{mol}{\mathrm{kg}}^{-1}$ solution of ${\mathrm{K}}_2{\mathrm{SO}}_4$ is: (Assume complete dissociation of the electro …

A solution containing 62 g ethylene glycol in 250 g water is cooled to $-10^{\circ }\mathrm{C}$. If ${\mathrm{K}}_{\mathrm{f}}$ for water is $1.86{\mathrm{K}\mathrm{kg}\mathrm{mol}}^{-1}$, the amount of water(in g) separated as ice is

Which one of the following statements regarding Henry's law is not correct?

At room temperature, a dilute solution of urea is prepared by dissolving 0.60 g of urea in 360 g of water. If the vapour pressure of pure water at this temperature is 35 mm Hg, lowering of vapour pressure will be: (molar mass of urea $=60\mathrm{g}{\mathrm{mol}}^{-1}$)

For 1 molal aqueous solution of the following compounds, which one will show the highest freezing point ?

The freezing point of benzene decreases by $0.45^{\circ }\mathrm{C}$ when 0.2 g of acetic acid is added to 20 g of benzene. If acetic acid associates to form a dimer in benzene, percentage association of acetic acid in benzene will be :
$({\mathrm{K}}_{\mathrm{f}}$ for benzene …

18 g glucose $(\mathrm{C}{}_6\mathrm{H}{}_{12}\mathrm{O}{}_6)$ is added to 178.2 g water. The vapour pressure of water (in torr) for this aqueous solution is :

The vapour pressure of acetone at $20^{\circ }\mathrm{C}$ is 185 torr. When 1.2 g of a non-volatile substance was dissolved in 100 g of acetone at $20^{\circ }\mathrm{C}$, its vapour pressure was 183 torr. The molar mass $(\mathrm{g}{\mathrm{mol}}^{-1})$ of the substance is:

Consider separate solutions of $0.500\mathrm{M}{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}(\mathrm{aq}),0.100\mathrm{M}{\mathrm{Mg}}_3({\mathrm{PO}}_4{)}_2(\mathrm{aq}),0.250\mathrm{M}\mathrm{KBr}(\mathrm{aq})$ and 0.125 …

${\mathrm{K}}_{\mathrm{f}}$ for water is $1.86\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}$. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol $\left({\mathrm{C}}_2{\mathrm{H}}_6{\mathrm{O}}_2\right)$ must you add to get the freezing point …

The degree of dissociation ( $\alpha$ ) of a weak electrolyte, $A_x{B}_y$ is related to van't Hoff factor (i) by the expression :

Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at $-6^{\circ }\mathrm{C}$ will be : [ ${\mathrm{K}}_{\mathrm{f}}$ for water $=1.86\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}$, an …

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water $(\Delta {\mathrm{T}}_{\mathrm{f}})$, when 0.01 mol of sodium sulphate is dissolved in 1 kg of water, is ( …

On mixing, heptane and octane form an ideal solution. At 373 K, the vapour pressures of the two liquid components (heptane and octane) are 105 kPa and 45 kPa respectively. Vapour pressure of the solution obtained by mixing 25.0 g of heptane and 35 g of octane will be (molar mass …

Two liquids X and Y form an ideal solution. At 300 K , vapour pressure of the solution containing 1 mol of $X$ and 3 mol of $Y$ is 550 mm Hg . At the same temperature, if 1 mol of $Y$ is further added to this solution, vapour pressure of the solution increases by 10 mm Hg . …

A binary liquid solution is prepared by mixing $n$-heptane and ethanol. Which one of the following statements is correct regarding the behaviour of the solution ?

At $80^{\circ }\mathrm{C}$, the vapour pressure of pure liquid ' $A$ ' is 520 mm Hg and that of pure liquid ' $B$ ' is 1000 mm Hg . If a mixture solution of ' A ' and ' B ' boils at $80^{\circ }\mathrm{C}$ and 1 atm pressure, the amount of ' A ' in the mixture is ( …

The vapour pressure of water at $20^{\circ }\mathrm{C}$ is 17.5 mm Hg. If 18 g of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ is added to 178.2 g of water at $20^{\circ }\mathrm{C}$, the vapour pressure of the resulting solution will be

A $5.25\%$ solution of a substance is isotonic with a $1.5\%$ solution of urea (molar mass $=60\mathrm{g}{\mathrm{mol}}^{-1}$) in the same solvent. If the densities of both the solutions are assumed to be equal to $1.0\mathrm{g}{\mathrm{cm}}^{-3}$, molar mass of the substance …

A mixture of ethyl alcohol and propyl alcohol has a vapour pressure of 290 mm at 300 K . The vapour pressure of propyl alcohol is 200 mm . If the mole fraction of ethyl alcohol is 0.6 , its vapour pressure (in mm ) at the same temperature will be

18 g of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ is added to 178.2 g of water. The vapour pressure of water for this aqueous solution at $100^{\circ }\mathrm{C}$ is

If $\alpha$ is the degree of dissociation of ${\mathrm{Na}}_2{\mathrm{SO}}_4$, the vant Hoff's factor (i) used for calculating the molecular mass is

Benzene and toluene form nearly ideal solutions. At $20^{\circ }$ C, the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The partial vapour pressure of benzene at $20^{\circ }$ C for a solution containing 78 g of benzene and 46 g of toluene in torr is

Equimolar solutions in the same solvent have

Which one of the following aqueous solutions will exhibit highest boiling point?

Which of the following liquid pairs shows a positive deviation from Raoult's law?

Which one of the following statements is false?
(1) Raoult's law states that the vapour pressure of a components over a solution is proportional to its mole fraction
(2) Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depres …