Solutions practice · Medium

What is the amount of $\mathrm{CaCl}_2(\mathrm{i}=2.9)$ dissolved in 4 litre of water such that its osmotic pressure is 1 atm at $27^{\circ} \mathrm{C}$?

Which of the following statements is incorrect?

Which of the following will have the highest boiling point at $1 {~atm}$ pressure

Calculate the mole fractions of the components of the solution composed by $92 \mathrm{~g}$ glycerol and $90 \mathrm{~g}$ water$? \, \, (M$ (water$)=18 ; M($glycerol$)=92)$

Statement I: Molarity of $0.02 \mathrm{~N} \mathrm{~HNO}_3$ is $0.02 \mathrm{~M}$.

Statement II: Molarity and normality of a solution are always same.

Percent by mass of solute (molar mass $=25 \mathrm{~g} / \mathrm{mol}$ ) in its aqueous solution is 30 . The mole fraction and molality of the solute in solution are

The vapour pressure of a pure liquid A is 40 mm Hg at 310 K. The vapour pressure of this liquid in a solution with liquid B is 32 mm Hg. What is the mole fraction of A in the solution if it obeys the Raoult’s law?

When 45 gm solute is dissolved in 600 gm water freezing point lower by 2.2 K, calculate molar mass of solute $\left( {{K_f} = 1.86\,K\,kg} \right)$

The boiling point elevation constant for toluene is $3.32 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. The normal boiling point of toluene is $110.7^{\circ} \mathrm{C}$. The enthalpy of vaporisation of toluene would be nearly:

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:

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?

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 $= 62\;g\mathrm{ }\;mo{l^{ - 1}}$

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

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

$0.48 \mathrm{~g}$ 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?