Solutions practice · Mixed difficulty

Mole fraction of $A$ vapours above the solution in mixture of ${A}$ and ${B}\left({X}_{{A}}=0.4\right)$ will be
[Given: ${P}_{{A}}^0=100 {~mm} {Hg}$ and ${P}_{{B}}^0=200 {~mm} {Hg}$ ]

What is the mole fraction of the solute in a 2.00 m aqueous solution :

A solution of acetone in ethanol

If osmotic pressure of $4 \%(\mathrm{w} / \mathrm{v})$ solution of sucrose is same as $2 \%(\mathrm{w} / \mathrm{v})$ solution of ' $\mathrm{X}$ ' find molecular mass of $\mathrm{X}$.

Which statement is not correct if two immiscible liquids of mol. wt. A and B respectively are mixed in equal amount to have a mixture?

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water $\Delta {T_f}$, when 0.01 mole of sodium sulphate is dissolved in 1 kg of water, is $({k_f} = 1.86\;\mathrm{K}\;\mathrm{kg mo}{\mathrm{l}^{ - 1}})$

Assertion (A) : At equilibrium of Liquid $\rightleftharpoons$ Vapour, kinetic energy of liquid phase and vapour phase is same.

Reason (R) : Kinetic energy of liquid or vapour is given by $\frac{3}{2} R T$ for 1 mole.

Consider the following statements.

I. The ${P}_{{H}}$ of a mixture containing $400\, {ml}$ of $0.1 {M} \,{H}_2 {SO}_4$ and $400 \,{ml}$ of $0.1 \,{M}\, {NaOH}$ will be approximately 1.3

II. Ionic product of water is temperature dependent

III. Le-chatelier's principle is applicable to common-ion effect

IV. A mixture of ${HClO}_4+{NaClO}_4$ acts as an acidic buffer.

The correct statements are

Assertion: There will not be any change in concentration of an ethanol and water mixture containing $85 \%$ ethanol by volume on boiling.

Reason: It is because azeotropes boil out in constant composition.

$1 \mathrm{~kg}$ of water under a nitrogen pressure of 1 atmosphere dissolves $0.02 \mathrm{~gm}$ of nitrogen at 293 K. Calculate Henry's law constant :

Assertion : Molarity of 0.02 N solution of $\mathrm{HNO}_3$ is 0.02 M

Reason : Molarity and Normality of a solution are always equal for any acid.

The freezing point of equilibrium solution in aqueous medium will be highest for

Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).
Assertion (A): At $10^\circ C,$ the density of a 5 M solution of $KCl$ [atomic masses of $K\,\,\& \,\,Cl$ are 39 & 35.5 $g\,\,mo{l^{ - 1}}$ respectively] is $'x'\,\,g\,\,m{l^{ - 1}}.$ The solution is cooled to $- 21^\circ C.$ The molality of the solution will remain unchanged.
Reason (R) : The molality of a solution does not change with temperature as mass remains unaffected with temperature.
In the light of the above statements, choose the correct answer from the options given below.

Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by $0.2\,^\circ C.$ The percentage association of solute A in water is:
[Given: Molar mass of ${\text{A}} = 93\,\,g\,mo{l^{ - 1}}.$ Molal depression constant of water is $1.86\,K\,kg\,mo{l^{ - 1}}.]$

Calculate the mass percentage of aspirin $\left(\mathrm{C}_9 \mathrm{H}_8 \mathrm{O}_4\right)$ in acetonitrile $\left(\mathrm{CH}_3 \mathrm{CN}\right)$ when $6.5 \mathrm{~g}$ of $\mathrm{C}_9 \mathrm{H}_8 \mathrm{O}_4$ is dissolved in $450 \mathrm{~g}$ of $\mathrm{CH}_3 \mathrm{CN}$.

The lowering in vapour pressure caused by the addition of $100 \mathrm{~g}$ of sucrose (molecular mass $=342$) to $1000 \mathrm{~g}$ of lowering in water, if the vapour pressure of pure water at $25^{\circ} \mathrm{C}$ is $23.8 \mathrm{~mm} \mathrm{~Hg}$, is

Assertion (A): Respiratory apparatus of scuba divers contain a mixture of ${N}_2+{O}_2+{He}$

Reason (R): Solubility of nitrogen in blood is less than that of Helium

The distribution coefficient of ${\mathrm{I}_2}$ in between $\mathrm{CC}{\mathrm{l}_4}$ and ${\mathrm{H}_2}\mathrm{O}$ is 85 in favour of $\mathrm{CC}{\mathrm{l}_4}$ at $25^\circ \mathrm{C}$. If solubility of ${\mathrm{I}_2}$ in ${\mathrm{H}_2}\mathrm{O}$ at $25^\circ \mathrm{C}$ is 0.33 g $\mathrm{litr}{\mathrm{e}^{ - 1}},\mathrm{the \;solubility\; of}\,{\mathrm{I}_2}$ in $\mathrm{CC}{\mathrm{l}_4}$ is ……..g $\mathrm{litr}{\mathrm{e}^{ - 1}}$.

Solubility of deliquescent substances in water is generally :

Equal weight of a solute are dissolved in equal weight of two solvents $A$ and $B$ and formed very dilute solution. The relative lowering of vapour pressure for the solution $B$ has twice the relative lowering of vapour pressure for the solution $A$. If $M_A$ and $M_B$ are the molecular weights of solvents $A$ and $B$ respectively, then:

Solution A contains 7 g/L of $MgC{l_2}$ and solution B contains 7 g/L of $NaCl$. At room temperature, the osmotic pressure of

The vapour pressure of a solution at $373 {~K}$ is $700 {~mm}$ of ${Hg}$. The molality and mole fraction of solute in solution is:

An aqueous solution of a non-electrolyte boils at $100.52^{\circ} {C}$. The freezing point of the solution will be

Assertion (A): The depression in freezing point depends on the amount of the solute and nature of solvent.

Reason (R): For aqueous solutions of different electrolytes, molal depression constant will have different value.

An example of a solution having liquid in gas is:

A solution containing 500 g of a protein per litre is isotonic with a solution containing 3.42 g of sucrose per litre. The molecular mass of protein is :

The azeotropic mixture of water and ethonal boils at $78.15^{\circ} \mathrm{C}$. When this mixture is distilled, it is possible to obtain:

A solution of an organic compound develops an osmotic pressure of $2.07 \times 10^{-2} {Nm}^{-2}$. If the density of solution is $0.88 {~g} {dm}^{-3}$, the height which it will develop on separating with its solvent through semipermeable membrane is :

The use of common salts, e.g. $NaCl{\text{ or}}\,CaC{l_2}$ anhydrous is made to clear snow on the roads. This causes:

Assertion (A): For two solutions, $0.1 \mathrm{~m}$ aqueous solution of glucose and $0.1 \mathrm{~m}$ acetic acid in benzene, the lowering of vapour pressure is same.

Reason (R): Vapour pressure is always lowered when non-volatile solute is added to water.