Solutions PYQs

Mixture of chloroform and acetone forms a solution with negative deviation from Raoult’s law due to:

Match List-I with List-II Choose the correct answer from the options given below :

Which of the following aqueous solution will exhibit highest boiling point?

5 moles of liquid X and 10 moles of liquid Y make a solution having a vapour pressure of 70 torr. The vapour pressures of pure X and Y are 63 torr and 78 torr respectively. Which of the following is true regarding the described solution?

The Henry’s law constant (K$_H$) values of three gases A, B, C in water are 145, 2×10⁻⁵ and 35 kbar respectively. The solubility of these gases in water follows:

The plot of osmotic pressure (Π) vs concentration (mol L⁻¹) for a solution gives a straight line with slope 25.73 L bar mol⁻¹. The temperature at which the osmotic pressure measurement is done is: (Use R = 0.083 L bar mol⁻¹ K⁻¹)

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R. Assertion A : Helium is used to dilute oxygen in diving apparatus. Reason R : Helium has high solubility in O₂. In the light of the above statements, choose the correct answer from the options given below:

In one molal solution that contains 0.5 mole of a solute, there is:

The following solutions were prepared by dissolving $10\,g$ of glucose $(C_6H_{12}O_6)$ in $250\,mL$ of water $(P_1)$, $10\,g$ of urea $(CH_4N_2O)$ in $250\,mL$ of water $(P_2)$ and $10\,g$ of sucrose $(C_{12}H_{22}O_{11})$ in $250\,mL$ of water $(P_3)$. The right option for the decreasing order of osmotic pressure of these solutions is:

The correct option for the value of vapour pressure of a solution at 45°C with benzene to octane in molar ratio 3:2 is: [At 45°C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume ideal gas]

The freezing point depression constant (Kf) of benzene is 5.12 K kg mol⁻¹. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):

A mixture of N$_2$ and Ar gases in a cylinder contains 7 g of N$_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of N$_2$ is: [Use atomic masses (in g mol⁻¹): N = 14, Ar = 40]

The mixture which shows positive deviation from Raoult’s law is

The correct option representing a Freundlich adsorption isotherm is:

The density of 2 M aqueous solution of NaOH is 1.28 g/cm³. The molality of the solution is [Given that molecular mass of NaOH = 40 g mol⁻¹]

The molar solubility of $CaF_2\,(K_{sp}=5.3\times10^{-11})$ in $0.1\,M$ solution of NaF is:

Which of the following statements is correct regarding a solution of two components A and B exhibiting positive deviation from ideal behaviour?

In water saturated air, the mole fraction of water vapour is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is:

If molality of the dilute solution is doubled, the value of molal depression constant (K$_f$) will be

Which of the following is dependent on temperature?

The coagulation values in millimoles per litre of the electrolytes used for the coagulation of $As_2S_3$ are given below: I. $(NaCl)=52$ II. $(BaCl_2)=0.69$ III. $(MgSO_4)=0.22$ The correct order of their coagulating power is:

The van't Hoff factor $(i)$ for a dilute aqueous solution of the strong electrolyte barium hydroxide is:

Which one of the following is incorrect for ideal solution?

What is the mole fraction of the solute in a 1.00 m aqueous solution?

Of the following 0.10 M aqueous solutions, which one will exhibit the largest freezing point depression?

How many grams of concentrated nitric acid solution should be used to prepare $250\,mL$ of $2.0\,M\;HNO_3$? The concentrated acid is $70\%\;HNO_3$.

$6.02 \times 10^{20}$ molecules of urea are present in $100\,mL$ of its solution. The concentration of solution is

Vapour pressure of chloroform (CHCl₃) and dichloromethane (CH₂Cl₂) at 25°C are 200 mmHg and 41.5 mmHg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of CHCl₃ and 40 g of CH₂Cl₂ at the same temperature will be:

A 0.1 molal aqueous solution of a weak acid is 30% ionised. If $K_f$ for water is $1.86^\circ$ C/m, the freezing point of the solution will be:

200 mL of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at 300 K is found to be $2.57 \times 10^{-3}$ bar. The molar mass of protein will be (R = 0.083 L bar mol$^{-1}$ K$^{-1}$):

The equivalent conductance of $\dfrac{M}{32}$ solution of a weak monobasic acid is $8.0\;mho\;cm^2$ and at infinite dilution is $400\;mho\;cm^2$. The dissociation constant of this acid is:

A $0.0020\,M$ aqueous solution of an ionic compound $Co(NH_3)_5(NO_2)Cl$ freezes at $-0.00732^\circ C$. Number of moles of ions which $1$ mole of ionic compound produces on being dissolved in water will be: ($k_f$ = 1.86 °C/m)

The sequence of ionic mobility in aqueous solution is

A solution containing 10 g per dm³ of urea (molecular mass = 60 g mol⁻¹) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is:

1.00 g of a non-electrolyte solute (molar mass 250 g mol⁻¹) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K$_f$ of benzene is 5.12 K kg mol⁻¹, the freezing point of benzene will be lowered by:

A solution of acetone in ethanol:

During osmosis, flow of water through a semi-permeable membrane is:

The vapour pressure of two liquids P and Q are $80$ torr and $60$ torr respectively. The total vapour pressure of solution obtained by mixing $3$ moles of P and $2$ moles of Q would be:

A solution of urea (molar mass $56\ g\ mol^{-1}$) boils at $100.18^{\circ}C$ at atmospheric pressure. If $K_f$ and $K_b$ for water are $1.86$ and $0.512\ K\ kg\ mol^{-1}$ respectively, the above solution will freeze at:

A solution has a $1:4$ mole ratio of pentane to hexane. The vapour pressure of pure hydrocarbons at $20^{\circ}C$ are $440\ mm\ Hg$ for pentane and $120\ mm\ Hg$ for hexane. The mole fraction of pentane in the vapour phase would be:

The mole fraction of the solute in one molal aqueous solution is: