Elements $X$ and $Y$ form two non-volatile compounds ( $X Y$ and $X Y_3$ ). When 10 g of $X Y$ is dissolved in 50 g of ethanol, the depression in freezing point ( $\Delta T_f$ ) was 5.333 K . When 10 g of $X Y_3$ is dissolved in 50 g of ethanol, the (was $\left.\Delta T_f\right) 2.2857 \mathrm{~K}$. What are the atomic weights of $X$ and $Y$ respectively?

$ \left(K_f=2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right) $

A solution is prepared by adding 124 g of ethylene glycol (molar mass $=62 \mathrm{~g} \mathrm{~mol}^{-1}$ ) to $x \mathrm{~g}$ of water to get 10 m solution. What is the value of $x$ (in g )?

The following graph is obtained for an ideal solution containing a non-volatile solute $x$-and $y$-axis represent, respectively

What is the approximate molality of $10 \%(w / w)$ aqueous glucose solution?

(Molar mass of glucose $=180 \mathrm{~g} \mathrm{~mol}^{-1}$ )

The van't Hoff factor for 0.5 m aqueous $\mathrm{CH}_2 \mathrm{FCOOH}$ solution is 1.075 . What is the experimentally observed $\Delta T_f$ (in K ) for this solution?

( $K_f=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ )

An aqueous solution containing 0.2 g of a non volatile solute ' $A$ ' in 21.5 g of water freezes at 272.814 K . If the freezing point of water is 273.16 K , the molar mass (in $\mathrm{g} \mathrm{mol}^{-1}$ ) of solute $A$ is $\left[\mathrm{K}_f\left(\mathrm{H}_2 \mathrm{O}\right)=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

At $T(\mathrm{~K})$, the vapour pressure of $x$ molal aqueous solution containing a non-volatile solute is $12.078 \mathrm{kPa}_{\mathrm{d}}$, The vapour pressure of pure water at $T(\mathrm{~K})$ is 12.3 kPa . What is the value of $x$ ?

In aqueous glucose solution, the mole fraction of wate is 40 times to mole fraction of glucose. What is the weight percentage $(w / w)$ of glucose in the solution?

Benzoic acid molecules undergo dimerisation in benzene. 2.44 g of benzoic acid when dissolved in 30 g of benzene caused depression in freezing point of 2 K . What is the percentage of association of it?

(Given $K_f\left(\mathrm{C}_6 \mathrm{H}_6\right)=5 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$; molar mass of benzoic acid $=122 \mathrm{~g} \mathrm{~mol}^{-1}$ )

At $T(\mathrm{~K})$, the vapour pressure of pure benzene and toluene are 75 and 22 mm Hg respectively. 23.4 g of benzene and 64.4 g of toluene are mixed to form an ideal solution. If the vapours are in equilibrium with the liquid mixture, the mole fraction of toluene in vapour phase (At.wt. of $\mathrm{C}=12, \mathrm{H}=1$ )

1.95 g of non-volatile and non-electrolyte solute dissolved in 100 g of benzene lowered the freezing point of it by 0.64 K .

The molar mass of the solute (in $\mathrm{g} \mathrm{mol}^{-1}$ )

$ \left(K_f\left(\mathrm{C}_6 \mathrm{H}_6\right)=5.12 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right) $

At $298 \mathrm{~K}, 0.714$ moles of liquid $A$ is dissolved in 5.555 moles of liquid $B$. The vapour pressure of the resultant solution is 475 torr. The vapour pressure of pure liquid $A$ at the same temperature is 280.7 torr. What is the vapour pressure of pure liquid $B$ in torr?

The mole fractions of glucose and water in aqueous glucose solution are 0.0244 and 0.9756 respectively. What is the weight percentage $(w / w)$ of glucose in this solution?

At $T(\mathrm{~K})$, the vapour pressure of an aqueous solution of a non-volatile solute, whose mole fraction is 0.02 is found to be 34.65 mm Hg . What is the vapour pressure (in mm Hg ) of pure water at the same temperature?

A centi molar solution of acetic acid is $50 \%$ dissociated at $27^{\circ} \mathrm{C}$. The osmotic pressure of the solution (in atm ) is $\left(R=0.083 \mathrm{~L}\right.$ atm $\left.\mathrm{K}^{-1} \mathrm{~mol}^{-1}\right)$

At 300 K vapour pressure of a pure liquid. ' $A$ ' is 70 mm Hg . It forms an ideal solution with another liquid ' $B$ '. The mole fraction of $B$ in the solution is 0.2 and total vapour pressure of solution is 84 mm Hg at same temperature. What is the vapour pressure (in mm ) of pure liquid $B$ at 300 K ?

248 g of ethylene glycol $\left(\mathrm{C}_2 \mathrm{H}_6 \mathrm{O}_2\right)$ is added to 200 g of water to prepare antifreeze. What is the molality of resultant solution?

$ (\mathrm{C}=12 \mathrm{u} ; \mathrm{H}=1 \mathrm{u} ; \mathrm{O}=16 \mathrm{u}) $

A solution containing 7.5 g of urea (molar mass $=60 \mathrm{~g} \mathrm{~mol}^{-1}$ ) in 1 kg of water freezes at the same temperature as another solution containing 15 g of solute $X$, in the same amount of water. The molar mass of $X\left(\mathrm{~g} \mathrm{~mol}^{-1}\right)$ is

Two statements are given below

Statements I : Liquids $A$ and $B$ form a non-ideal solution with positive deviation. The interactions between $A$ and $B$ are weaker than $A-A$ and $B-B$ interactions.

Statements II : For an ideal solution $\Delta_{\text {mix }} H=0$; $\Delta_{\text {mix }} V=0$

The correct answer is

At 290 K , a vessel (I) contains equal moles of three liquids $(A, B, C)$. The boiling points of $A, B$ and $C$ are $350 \mathrm{~K}, 373 \mathrm{~K}$ and 308 K respectively. Vessel (I) is heated to 300 K and vapours were collected into vessel (II). Identify the correct statements. (Assume vessel (I) contains liquids and vapours and vessel (II)contains only vapours)

(I) Vessel - I is rich in liquid $B$

(II) Vessel - II is rich in vapour of $C$

(III) The vapour pressures of $A, B, C$ in vessel (I) at 290 K follows the order $C>A>B$

At $300 \mathrm{~K}, 6 \mathrm{~g}$ of urea was dissolved in 500 mL of water. What is the osmotic pressure (in atm) of resultant solution?

$ \begin{aligned} & \left(R=0.082 \mathrm{~L}^{\operatorname{atm~K}}{ }^{-1} \mathrm{~mol}^{-1}\right) \\ & (\mathrm{C}=12 ; \mathrm{N}=14 ; \mathrm{O}=16 ; \mathrm{H}=1) \end{aligned} $

Benzoic acid undergoes dimerisation in benzene. $x \mathrm{~g}$ of benzoic acid (molar mass $122 \mathrm{~g} \mathrm{~mol}^{-1}$ ) is dissolved in 49 g of benzene. The depression in freezing point is 1.12 K . If degree of association of acid is $88 \%$. What is the value of $x$ ? $\left(K_f\right.$ for benzene $\left.=4.9 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

At $T(\mathrm{~K})$ two liquids $A$ and $B$ form an ideal solution. The vapour pressures of pure liquid $A$ and $B$ at that temperature are 400 and 600 mm Hg respectively, If the mole fraction of liquid $B$ is 0.3 in the mixture, the mole fractions of $A$ and $B$ in vapour phase respectively are

The following graph is obtained for vapour pressure (in atm) (on $Y$-axis) and $T$ (in K) (on $X$-axis) for aqueous urea solution and water. What is the boiling point (in K) of urea solution?

(Atmospheric pressure $=1 \mathrm{~atm}$ )

Given below are two statements.

Statement I : Liquids $A$ and $B$ form a non-ideal solution with negative deviation. The interactions between $A$ and $B$ are weaker than $A-A$ and $B-B$ interactions.

Statement II : In reverse osmosis, the applied pressure must be higher than the osmotic pressure of solution

The correct answer is

A non- volatile solute is dissolved in water. The $\Delta T_{\mathrm{b}}$ of resultant solution is 0.052 K . What is the freezing point of the solution ( in K )?

( $K_b$ of water $=0.52 \mathrm{~K} \mathrm{kgmol}^{-1}$,

$K_f$ of water $=1.86 \mathrm{~K} \mathrm{kgmol}^{-1}$,

freezing point of water $=273 \mathrm{~K}$ )

The osmotic pressure of sea water is 1.05 atm . Four experiments were carried as shown in table. In which of the following experiments, pure water can be obtained in part-II of vessel.

0.05 mole of a non-volatile solute is dissolved in 500 g of water. What is the depression in freezing point of resultant solution?

$\left(K_f\left(\mathrm{H}_2 \mathrm{O}\right)=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

Which of the following form an ideal solution?

I. Chloroethane and bromoethane

II. Benzene and toluene

III. $n$-hexane and $n$-heptane

IV. Phenol and aniline

A solution containing 6.0 g of urea is isotonic with a solution containing 10 g of a non-electrolytic solute $X$. The molar mass of X (in g $\mathrm{mol}^{-1}$) is

$x \%(w / V)$ solution of urea is isotonic with $4 \%$ $(w / V)$ solution of a non-volatile solute of molar mass $120 \mathrm{~g} \mathrm{~mol}^{-1}$. The value of $x$ is

At $T(\mathrm{~K}) \times \mathrm{g}$ of a non-volatile solid (molar mass $78 \mathrm{~g} \mathrm{~mol}^{-1}$) when added to 0.5 kg water, lowered its freezing point by $1.0^{\circ} \mathrm{C}$. What is $x$ (in g)? ($K_f$ of water at $T(\mathrm{~K})=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$)

Assertion (A) Blood cells collapse when suspended in saline water.

Reason (R) Cell membrane dissolves in saline water.

If two liquids $A$ and $B$ form a minimum boiling azeotrope at some specific composition, then which statement among the following is correct?

The vapour pressure of a solvent decreased by 20 mm of Hg when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.5. What should be the mole fraction of the solvent for the decrease in the vapour pressure needs to be 10 mm of Hg?

If the $K_{\mathrm{H}}$ values for $\operatorname{Ar}(g), \mathrm{CO}_2(g), \mathrm{HCHO}(g)$ and $\mathrm{CH}_4(\mathrm{~g})$ respectively are $40.39,1.67, 1.83 \times 10^{-5}$ and $0.413$ , then identify the correct increasing order of their solubilities.

If 500 mL of CaCl$_2$ solution contains 3.01 $\times$ 10$^{22}$ chloride ions, molarity of the solution will be

Which condition is not satisfied by an ideal solution?

A solution of urea (molar mass $60 \mathrm{~g} \mathrm{~mol}^{-1}$ ) boils at $100.20^{\circ} \mathrm{C}$ at the atmospheric pressure, if $K_f$ and $K_b$ for water are 1.86 and $0.512 \mathrm{~K}$ $\mathrm{kg} \mathrm{mol}^{-1}$ respectively. The freezing point of the solution will be

When difference in boiling points of two liquids is too small, then the separation is carried out by

Which of the following will form an ideal solution?

The molal elevation constant is the ratio of elevation in boiling point to