Solutions practice · Mixed difficulty

If 0.2 m aqueous solution of ${K_4}\left[ {Fe{{\left( {CN} \right)}_6}} \right]$ is 100% ionized then the freezing point of the solution will be $\left( {{K_f} = 1.86\,K\,kg\,mo{l^{ - 1}}} \right)$

Given below are two statements:

Statement (I): NaCl is added to the ice at $0^{\circ} \mathrm{C},$ present in the ice cream box to prevent the melting of ice cream.

Statement (II): On addition of NaCl to ice at $0^{\circ} \mathrm{C},$ there is a depression in freezing point.

In the light of the above statements, choose the correct answer from the options given below:

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

Assertion: The mixing of two completely miscible liquids. A and B showing positive deviation from Raoult's law is followed by an absorption of heat

Reason: The A-B molecular interaction forces are stronger than the A-A or B-B molecular interaction forces.

Select correct statement ?

Which is an application of Henry's law?

How many mole of helium gas occupy $22.4 \mathrm{~L}$ at $0^{\circ} \mathrm{C}$ at 1 atm. Pressure

Assertion: After adding non-volatile solute freezing point of solvent depressed.

Reason: Vapour pressure of solvent decreases and become equal to solid solvent, at temperature lower than the freezing point of pure solvent.

Which has maximum freezing point ?

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 $({K_f}\;\mathrm{for}\;\mathrm{ water} = 1.86\;\mathrm{K}\;\mathrm{ kg }\;\mathrm{mo}{\mathrm{l}^{ - 1}}\mathrm{)}\mathrm{.}$ and molar mass of ethylene glycol $= 62\;g\mathrm{ }\;mo{l^{ - 1}}$

A 5 molar solution of ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ is diluted from 1 L to 10 L. What is the normality of the solution?

Isotonic solutions have same

In liquid ${CCl}_4$ which of the following has maximum solubility?

Molarity of $0.2\;N\;{H_2}S{O_4}$ is

Which of the following solution has highest freezing point?

What is the molality of pure water?

Calculate the osmotic pressure of $0.1 N {Na}_3 {PO}_4$ solution at $300 {~K}$.

The vapour pressure of a saturated solution of sparingly soluble salt $\left({XCl}_3\right)$ was $17.20 \mathrm{~mm} \mathrm{~Hg}$ at $27^{\circ} \mathrm{C}.$ If the vapour pressure of pure water is $17.25 \mathrm{~mm} \mathrm{~Hg}$ at $27^{\circ} \mathrm{C},$ then what is the solubility of the sparingly soluble salt ${XCl}_3$ in mole per litre?

When benzoic acid dissolve in benzene, the observed molecular mass is

$3.65\;g\;of\;\mathrm{HCl}$ is dissolved in $16.2\;g$ of water. The mole fraction of $\mathrm{HCl}$ in the resulting solution is

An azeotropic solution of two liquids has a boiling point lower than either of them when it:

A 5.25% solution of a substance is isotonic with a 1.5% solution of urea (molar mass $= 60\;g\;\mathrm{mo}{\mathrm{l}^{ - 1}}$) in the same solvent. If the densities of both the solutions are assumed to be equal to $\mathrm{1}\mathrm{.0}\;\mathrm{g}\;\mathrm{c}{\mathrm{m}^{ - 3}},$ molarmass of the substance will be

$0.48 \mathrm{~g}$ of a substance is dissolved in $10.6 \mathrm{~g}$ of $\mathrm{C}_6 \mathrm{H}_6.$ The freezing point of benzene is lowered by $1.8^{\circ} \mathrm{C}.$ What will be the molecular weight of the substance $\left(K_{\mathrm{f}} \text{ for benzene}=5\right)?$

One mole each of urea, glucose and sodium chloride were dissolved in one litre of water Equal osmotic pressure will be produced by solutions of

Statement I: If cells of living organisms are placed in pure water, they swell and burst.

Statement II: Due to osmosis, the movement of water molecules into the cell dilutes the salt content.

Air was drawn through a solution containing $40 \mathrm{~g}$ of solute (non-volatile and non-electrolyte) in $100 \mathrm{~g}$ of water and then through water. The loss of mass of water was $0.05 \mathrm{~g}$ and the total mass of water absorbed in sulphuric acid tube was $2.05 \mathrm{~g}.$ The molecular mass of the solute is

$24 {~g}$ of difluoroacetic acid in $400 \,{~g}$ of water has observed freezing point depression by $1.4 \,{~K}$. The van't Hoff factor for difluoroacetic acid is
$\left({K}_{{f}}\right.$ of water $=1.86 \,{~K}\, {~kg} {~mol}^{-1}$; Atomic weight of ${F}=19$ )

AN aqueous solution is 1.00 $\,$ molal in $\,{KI}$. Which change will cause the vapour pressure of the solution to increase?

What is the composition of gases in the tanks used by the scuba divers?

Van't Hoff factor for the aqueous solution of $\mathrm{AlCl}_3$ is 2.8. The percentage dissociation of $\mathrm{AlCl}_3$ is: