Solutions practice · Medium

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

One gram of silver gets distributed between $10{\kern 1pt} \,\mathrm{c}{\mathrm{m}^3}$ of molten zinc and $100\,\mathrm{c}{\mathrm{m}^3}$ of molten lead at $8000^\circ C.$ The percentage of silver still left in the lead layer in approximately

A solution of sodium sulphate contains 92 g of $N{a^ + }$ ions per kilogram of water. The molality of $N{a^ + }$ ions in that solution in $mol\;k{g^{ - 1}}$ is

What volume of $10 \mathrm{~M} \mathrm{~HCl}$ and $3 \mathrm{~M} \mathrm{~HCl}$ should be mixed to get $1 \mathrm{~L}$ of $6 \mathrm{~M} \mathrm{~HCl}$ solution?

The modal elevation constant of water is $0.52^\circ \mathrm{C}$ . The boiling point of 1.0 modal aqueous KCl solution (assuming complete dissociation of KCl), therefore, should be

Statement I: In solution different parts show different composition.

Statement II: Solution is homogeneous mixture.

At a given temperature, osmotic pressure of the concentrated solution of a substance

For a solution of $0.849 \mathrm{~g}$ of mercurous chloride in $50 \mathrm{~g}$ of $\mathrm{HgCl}_2(\ell)$ the freezing point depression is $1.24^{\circ} \mathrm{C}$. $\mathrm{K}_{\mathrm{f}}$ for $\mathrm{HgCl}_2$ is 34.3. What is the state of mercurous chloride in $\mathrm{HgCl}_2$ ? $(\mathrm{Hg}-200, \mathrm{Cl}-35.5)$

Which of the following compounds can be used as antifreeze in automobile radiators?

STATEMENT-1 : Osmotic pressure is a colligative property.

STATEMENT-2 : Osmotic pressure developed in a column due to osmosis.

Statement II: The vapour pressure of $0.1 \mathrm{M}$ sugar solution is more than that of $0.1 \mathrm{~M} \mathrm{~KCl}$ solution.

Statement II: Lowering of vapour pressure is directly proportional to the number of species present in the solution.

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 :

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 $\mathrm{X}$.

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

$1 \mathrm{~kg}$ 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.

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 $\mathrm{CH}_3 \mathrm{CN}$.

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

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

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.

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 :

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.

The correct option for the value of vapour pressure of a solution at ${45^0}C$ with benzene to octane in molar ratio $3:2$ is
[At ${45^0}C$ vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume ideal gas]

Which will have largest $\Delta {T}_{{b}}?$

Which relation is incorrect for a solution that shows positive deviation from Raoult's law?