Solutions

Two volatile liquids $\mathbf{A}$ and $\mathbf{B}$ form an ideal solution. Consider a 5 molal solution of $\mathbf{B}$ in $\mathbf{A}$ inside a closed container having a total vapour pressure of 100 mm Hg at 300 K . The vapour pressure of p...

Two volatile liquids $\mathbf{A}$ and $\mathbf{B}$ form an ideal solution. Consider a 5 molal solution of $\mathbf{B}$ in $\mathbf{A}$ inside a closed container having a total vapour pressure of 100 mm Hg at 300 K . The vapour pressure of p...

In a solvent $\mathbf{S}$, a compound $\mathbf{B}$ is partially dissociated into $\mathbf{C}$ and $\mathbf{D}$ as given below :
\(\mathbf{B} \rightleftharpoons 2 \mathbf{C}+2 \mathbf{D}\)
$\mathbf{B}, \mathbf{C}$ and $\mathbf{D}$ are non-...

At 300 K , an ideal dilute solution of a macromolecule exerts osmotic pressure that is expressed in terms of the height $(h)$ of the solution (density $=1.00 \mathrm{~g} \mathrm{~cm}^{-3}$ ) where $h$ is equal to 2.00 cm . If the concentrat...

Vessel-1 contains $\mathbf{w}_2 \mathrm{~g}$ of a non-volatile solute $\mathbf{X}$ dissolved in $\mathbf{w}_1 \mathrm{~g}$ of water. Vessel- 2 contains $\mathbf{w}_2 \mathrm{~g}$ of another non-volatile solute $\mathbf{Y}$ dissolved in $\ma...

$50 \mathrm{~mL}$ of 0.2 molal urea solution (density $=1.012 \mathrm{~g} \mathrm{~mL}^{-1}$ at $300 \mathrm{~K}$ ) is mixed with $250 \mathrm{~mL}$ of a solution containing $0.06 \mathrm{~g}$ of urea. Both the solutions were prepared in th...

An aqueous solution is prepared by dissolving $0.1 \mathrm{~mol}$ of an ionic salt in $1.8 \mathrm{~kg}$ of water at $35^{\circ} \mathrm{C}$. The salt remains $90 \%$ dissociated in the solution. The vapour pressure of the solution is $59.7...

The value of | y | is ________.

The value of x is ________.

Liquids A and B form ideal solution for all compositions of A and B at 25\(^\circ\)C. Two such solutions with 0.25 and 0.50 mole fractions of A have the total vapour pressure of 0.3 and 0.4 bar, respectively. What is the vapour pressure of...

On dissolving 0.5 g of a non-volatile non-ionic solute to 39 g of benzene, its vapor pressure decreases from 650 mmHg to 640 mmHg. The depression of freezing point of benzene (in K) upon addition of the solute is .............(Given data: M...

Liquids A and B form ideal solution over the entire range of composition. At temperature \(T,\) equimolar binary solution of liquids \(A\) and \(B\) has vapor pressure \(45\) \(Torr.\) At the same temperature, a new solution of \(A\) and ...

The plot given below shows \(P-T\) curves (where \(P\) is the pressure and \(T\) is the temperature) for two solvents \(X\) and \(Y\) and isomolal solutions of \(NaCl\) in these solvents. \(NaCl\) completely dissociates in both the solvents...

Pure water freezes at \(273\) \(K\) and \(1\) bar. The addition of \(34.5\) \(g\) of ethanol to \(500\) \(g\) of water changes the freezing point of the solution. Use the freezing point depression constant of water as \(2\) kg $$mo{l^{ - 1}...

For a solution formed by mixing liquids \(L\) and \(M,\) the vapor pressure of \(L\) plotted against the mole fraction of \(M\) in solution is shown in the following figure. Here \({X_L}\) and \({X_M}\) represent mole fractions of \(L\) and...

Mixture (s) showing positive deviation from Raoult’s law at 35oC is (are)

The qualitative sketches I, II and III given below show the variation of surface tension with molar concentration of three different aqueous solutions of KCl, CH3OH and CH3(CH2)11 OSO\(_3^ -\) Na+ at room temperature. The correct assignmen...

The mole fraction of a solute in a solution is 0.1. At 298 K, molarity of this solution is the same as its
molality. Density of this solution at 298 K is 2.0 g cm–3 . The ratio of the molecular weights of the solute and solvent, $$\left( {{...

If the freezing point of a 0.01 molal aqueous solution of a cobalt (III) chloride-ammonia complex(which
behaves as a strong electrolyte) is – 0.0558oC, the number of chloride(s) in the coordination sphere of the
complex is [Kf of water = 1....

MX2 dissociates in M2+ and X- ions in an aqueous solution, with a degree of dissociation (\(\alpha\)) of 0.5. The
ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of
freezing point in...

For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in 100 g of water. the elevation in boiling point at 1 atm pressure is 2oC. Assuming concentration of solute is much lower than the concentration of solvent, th...

The freezing point (in oC) of a solution containing 0.1 g of K3[Fe(CN)6] (Mol. wt. 329) in 100 g of water (Kf = 1.86 K kg mol-1) is

The Henry's law constant for the solubility of N\(_2\) gas in water at 298 K is 1.0 \(\times\) 10\(^5\) atm. The mole fraction of N\(_2\) in air is 0.8. The number of moles of N\(_2\) from air dissolved in 10 moles of water at 298 K and 5 a...

Water is added to the solution M such that the fraction of water in the solution becomes 0.9 mole. The boiling point of this solution is:

The vapour pressure of the solution M is :

The freezing point of the solution M is :

When 20 g of naphthoic acid (C\(_{11}\)H\(_{8}\)O\(_{2}\)) is dissolved in 50 g of benzene in 50 g of benzene (K\(_f\) = 1.72 K kg mol\(^{-1}\)), a freezing point depression of 2 K is observed. The van't Hoff factor (i) is :

75.2 g of C6H5OH (phenol) is dissolved in a solvent of Kf = 14. If the depression in freezing point is 7 K then find the % of phenol that dimerises.

The elevation in boiling point of a solution of 13.44 g of CuCl2 in 1kg of water using the following information will be (Molecular weight of CuCl2 = 134.4 and Kb = 0.52 K molal-1)

1.22 g of benzoic acid is dissolved in 100 g of acetone and 100 g of benzene separately. Boiling point of the solution in acetone increases by 0.17 oC, while that in the benzene increases by 0.13oC; Kb for acetone and benzene is 1.7 K kg m...

To 500 cm3 of water, 3.0 \(\times\) 10-3 kg of acetic acid is added. If 23% of acetic acid is dissociated, what will be the depression in freezing point? Kf and density of water are 1.86 K kg-1 mol-1 and 0.997 g cm-3, respectively

Nitrobenzene is formed as the major product along with a minor product in the reaction of benzene with a hot mixture of nitric acid and sulphuric acid. The minor product consists of carbon : 42.86 %, hydrogen : 2.40%, nitrogen : 16.67% and ...

A solution of a nonvolatile solute in water freezes at -0.30oC. The vapour pressure of pure water at 298 K s 23.51 mm Hg and Kf for water is 1.86 K kg mol-1. Calculate the vapour pressure of this solution at 298 K.

The molar volume of liquid benzene (density = 0.877 g mL-1) increases by a factor of 2750 as it vaporises at 20oC and that of liquid toluene (density = 0.867 g mL-1) increases by a factor of 7720 at 20oC. A solution of benzene and toluene a...

What weight of the non-volatile solute, urea(NH2 - CO - NH2) needs to be dissolved in 100g of water, in order to decrease the vapour pressure of water by 25%? What will be the molality of the solution?

The degree of dissociation of calcium nitrate in a dilute aqueous solution, containing 7.0 g. of the salt per 100 gm of water at 100oC is 70%. If the vapour pressure of water at 100oC is 760 mm, calculate the vapour pressure of the solution...

The freezing point of equimolal aqueous solutions will be highest for

The vapour pressure of pure benzene at a certain temperature is 640 mm Hg. A non-volatile non-electrolyte solid weighing 2.175 g is added to 39.0 g of benzene. The vapour pressure of the solution is 600 mm Hg. What is the molecular weight o...

The vapour pressure of a dilute aqueous solution of glucose (C6H12O6) is 750 mm of mercury at 373 K. Calculate (i) molality, and (ii) mole fraction of the solution.

The vapour pressure of ethanol and methanol are 44.5 and 88.7 mm Hg respectively. An ideal solution is formed at the same temperature by mixing 60 g of ethanol with 40 g of methanol. Calculate the total vapour pressure of the solution and t...

An organic compound CxH2yOy was burnt with twice the amount of oxygen needed for complete combustion of CO2 and H2O. The hot gases when cooled to 0oC and 1 atm pressure, measured 2.24 litres. The water collected during cooling weighed 0.9 g...

The vapour pressure of pure benzene is 639.7 mm of mercury and the vapour of a solution of a solute in benzene at the same temperature is 631.9 mm of mercury. Calculate this molality of the solution.