Solutions practice · Mixed difficulty

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]

Liquids 'A' and 'B' form an ideal solution. At $80^{\circ} \mathrm{C}, \mathrm{P}_{\mathrm{A}}^0=0.4 \mathrm{~bar}$ and $\mathrm{P}_{\mathrm{B}}^0=0.8 \mathrm{~bar}.$ All the vapour above the liquid solution containing equal moles of both the liquids at equilibrium is collected in another empty vessel and condensed. Now, the condesate is heated to $80^{\circ} \mathrm{C}$ and all the vapours above the liquid solution at equilibrium is again collected in another empty vessel and condensed. What is the mole-fraction of 'B' is new condensate?

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

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

The vapour pressure of $100 \mathrm{~g}$ water reduces from $17.53 \mathrm{~mm}$ to $17.22 \mathrm{~mm}$ when $17.10 \mathrm{~g}$ substance ' $X$ ' is dissolved in it. Substance $X$ can be

A solution containing $8.6 \mathrm{~g}$ urea in one litre was found to be isotonic with a $5 \%$ (mass/volume) solution of an organic non-volatile solute. The molar mass of solute is;

What weight of hydrated oxalic acid should be added for complete neutralisation of $100 \,{ml}$ of $0.2 {~N}-{NaOH}$ solution?

On dissolving $0.5 {~g}$ of a non-volatile non-ionic solute to $39 {~g}$ of benzene, its vapour 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..... K.
(Given data : Molar mass and the molal freezing point depression constant of benzene are $78 {~g} {~mol}^{-1}$ and $5.12 {~K} {~kg} {~mol}^{-1}$, respectively)

Which of the following mixture of solutions follow the condition $\Delta_{\text {mix }} H<0$ and $\Delta_{\text {mix }} V<0$ ?

(i) Nitric acid + Water

(ii) Acetic acid + Pyridine

(iii) Ethanol + Water

(iv) Carbon tetra chloride + Chloroform

$K_{s p}$ (solubility product) of $\mathrm{MgS}=\left(\mathrm{Mg}^{2+}\left(\mathrm{S}^{2-}\right)\right)$ is $1.0 \times 10^{-6}$. Thus, elevation in boiling point of saturated solution is $\left(K_b=0.52^{\circ} \mathrm{mol}^{-1} \mathrm{~kg}\right)$

The statement “the relative lowering of the vapour pressure is equal to th ratio ot moles of the solute to the total number of the moles in the solution” refers to

Among the following, the azeotropic mixture is

A liquid is kept in a closed vessel. If a glass plate (negligible mass) with a small hole is kept on top of the liquid surface, then the vapour pressure of the liquid in the vessel is :

Assertion : Camphor is used as solvent in the determination of molecular masses of naphthalene, anthracene etc.

Reason : Camphor has high molal elevation constant.

The relative lowering of vapour pressure is equal to the mole fraction of the non-volatile solute. This statement was given by:

Consider the following statements about osmotic pressure method of molar mass determination.

I. Molarity of the solution is used instead of molality.

II. Magnitude of osmotic pressure is very large even for dilute solutions.

III. Molar mass of biomolecules can be determined as they are not stable at higher temperatures.

IV. Determine the molar mass of polymer as they have poor solubility.

Which of the above statements are responsible for advantage of osmotic pressure for determination of molar mass over the other colligative properties?

Assertion (A) : Addition of solvent to a solution always lowers the V.P.

Reason (R) : The increase in relative surface area give rise to an increase in V.P. for a given solution.

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

According to Raoult's law, relative lowering of vapour pressure for a solution is equal to

Assertion: The molarity and normality of a solution of sodium carbonate are same.
Reason: Molarity is the product of normality &amp; valency factor.

How much water is needed to dilute $10 {~ml}$ of $10 {~N}$ hydrochloric acid to make it exactly decinormal $(0.1 {~N})$

Vapour pressure of pure water at $298 \mathrm{~K}$ is $23.8 \mathrm{~mm}$. Thus, vapour pressure of $20 \%$ glucose (weight/volume) solution is $\left(d=0.9971 \mathrm{~g} \mathrm{~mL}^{-1}\right)$

The freezing point of a solution containing $0.2 \mathrm{~g}$ of acetic acid in $20.0 \mathrm{~g}$ benzene is lowered by $0.45^{\circ} \mathrm{C}$. The degree of association of acetic acid in benzene is (Assume acetic acid dimerises in benzene and $\mathrm{K}_{\mathrm{f}}$ for benzene $=5.12 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$)
$\mathrm{M}_{\text {observed}}$ of acetic acid $=113.78$

The amount of ${K}_2 {Cr}_2 {O}_7$ (eq. wt. 49.04) required to prepare 100 ${ml}\,$ of its $0.05 {~N}$ solution is

The amino acid alanine has two isomers, such as
$\alpha-\text{alanine}$ and $\beta-\text{alanine}.$ When equal masses of
these two compounds are dissolved in equal mass
of a solvent, the solution of $\alpha-\text{alanine}$ freezes at
relatively lower temperature. Which forms of
$\alpha-\text{alanine}$ or $\beta-\text{alanine}$, has the larger equilibrium
constant for ionization?

S-I: The boiling point of $0.1 \, \mathrm{M}$ urea solution is less than that of $0.1 \, \mathrm{M} \, {KCl}$ solution.

S-II: Elevation of boiling point is directly proportional to the number of moles of non-volatile solute particles present in the solution.

The molarity of $24.5 \%$ (w/w) $\mathrm{H}_2 \mathrm{SO}_4$ solution having density $1.2 \mathrm{~g} / \mathrm{ml}$ is

Which of the following aqueous solution has minimum freezing point?

If the mass percentage $({w} / {w})$ of urea in aqueous solution is $18 \%$ then the molality of the solution is

Percentage ionization of ${K_3}\left[ {Fe{{\left( {CN} \right)}_6}} \right]$ whose decimolar solution shows an osmotic pressure of 3.94 atm at 300 K is