Liquid Solution

Calculate vapour pressure of volatile liquid A at given temperature if mole fraction and vapour pressure of volatile liquid B are 0.4 and 900 mm Hg respectively [ $\mathrm{P}_{\text {total }}=600 \mathrm{~mm} \mathrm{Hg}$ ]

Calculate the molality of the solution of nonvolatile solute if it freezes at $-0.36^{\circ} \mathrm{C}$.
$\left[K_{\mathrm{f}}\right.$ for solvent $\left.=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

Which of the following aqueous solutions having same molality exhibits maximum boiling point elevation? (Assume complete dissociation)

Calculate cryoscopic constant of solvent if depression in freezing point of 0.18 m solution of nonvolatile solute is 0.2 K

Calculate the mole fraction of pure liquid $B$ in solution if total vapour pressure of solution, vapour pressure of pure liquid A and vapour pressure of pure liquid B are 500 mm Hg , 400 mm Hg and 575 mm Hg respectively at given temperature...

Which from following pairs of solutions in water exhibits same osmotic pressure at same temperature?
[molar mass of urea $=60 \mathrm{~g} \mathrm{~mol}^{-1}$, sucrose $=342 \mathrm{~g} \mathrm{~mol}^{-1}$ ]

Calculate the molality of the solution containing nonvolatile solute if boiling point elevation of solution is 0.39 K .
[ $\mathrm{K}_{\mathrm{b}}$ of water $=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ ]

A solution of 5 g nonvolatile solute in 50 g water decreases its freezing point by 0.2 K . Calculate the molar mass of solute if $\mathrm{K}_{\mathrm{f}}$ of water is $1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$.

Arrange the following equimolar solutions according to increasing order of osmotic pressure [Assume complete ionisation]
i) KCl
ii) $\mathrm{BaCl}_2$
iii) $\mathrm{AlCl}_3$
iv) $\mathrm{Al}_2\left(\mathrm{SO}_4\right)_3$

Calculate the vapour pressure of solution if relative lowering of vapour pressure and vapour pressure of pure solvent are 0.018 and 18 mm Hg respectively at 300 K .

Calculate the number of moles of nonvolatile solute dissolved in 0.5 kg solvent if molal elevation constant for solvent is $2 \mathrm{~kg} \mathrm{~K} \mathrm{~mol}^{-1} \left[\Delta \mathrm{T}_{\mathrm{b}}=0.8 \mathrm{~K}\right]$

Calculate van't Hoff factor of aqueous solution of 0.18 m electrolyte that freezes at $-0.54^{\circ} \mathrm{C}$.
$\left(\mathrm{K}_{\mathrm{f}}\right.$ for solvent $\left.=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

Calculate the molality of solution of nonvolatile solute if boiling point elevation is 1.75 K .
[ $\mathrm{K}_{\mathrm{b}}$ for solvent $=3 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ ]

Determine the expected value of $\Delta T_f$ for $1 \mathrm{~m} \mathrm{CaCl}_2$ solution if 1 m urea solution has $\Delta \mathrm{T}_{\mathrm{f}}$ value ' $x$ ' K .

Calculate the cryoscopic constant of solvent if depression in freezing point of 0.4 m solution of nonvolatile solute is 1.8 K .

Which from following mixtures obeys Raoult's law?

Calculate the osmotic pressure of 0.2 M aqueous solution of electrolyte at 300 K . If van't Hoff factor is $1.6\left[\mathrm{R}=0.0821 \mathrm{~atm} \mathrm{dm} \mathrm{K}^{-1} \mathrm{~mol}^{-1}\right]$.

Calculate the osmotic pressure of 0.5 M aqueous solution of nonvolatile solute at 300 K .
\(\left[\mathrm{R}=0.0821 \mathrm{~atm} \mathrm{dm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]\)

Which from following mixtures exhibits positive deviation from Raoult's law?

Calculate the number of moles of nonvolatile solute dissolved in 0.3 kg solvent if $\Delta \mathrm{T}_{\mathrm{b}}=0.3 \mathrm{~K}$ and $\mathrm{K}_{\mathrm{b}}$ for solvent is $1.8 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$.

When 0.01 mole of nonvolatile solute is dissolved in certain solvent calculate the mass of solvent in kg if $\Delta \mathrm{T}_{\mathrm{b}}=0.6 \mathrm{~K}$ and $\mathrm{K}_{\mathrm{b}}$ for solvent= $2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol...

Which from following solutions exhibits minimum boiling point elevation under identical conditions? (Assume complete dissociation)

Calculate the relative lowering of vapour pressure of solution containing 3 g urea in 50 g water. [molar mass of urea $=60 \mathrm{~g} \mathrm{~mol}^{-1}$ ]

Which of the following aqueous solutions exhibits lowest freezing point depression assuming complete dissociation?

Calculate the temperature of 0.05 M sucrose solution in Kelvin if the osmotic pressure of the solution is 1.5 atm .
\(\left[\mathrm{R}=0.0821 \mathrm{dm}^3 \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]\)

Calculate molality of the solution containing nonvolatile solute if boiling point elevation of the solution is 0.2 K
\(\left[\mathrm{K}_{\mathrm{b}}=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]\)

Arrange the following solutions according to decreasing order of osmotic pressure under similar condition of temperature and assuming complete dissociation.
$$ \begin{array}{|c|l|} \hline \text { I. } & 0.2 \mathrm{~m} \mathrm{KCl} \\ \hlin...

Calculate the relative lowering of vapour pressure of solution containing 0.56 g nonvolatile solute in 100 g water [molar mass of solute $=60 \mathrm{~g} \mathrm{~mol}^{-1}$ ]

Calculate the boiling point elevation of solution if 15 g urea is dissolved in 1000 g water. $\left[\mathrm{K}_{\mathrm{b}}\right.$ for water $=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$; molar mass of urea $=60 \mathrm{~g} \mathrm{~...

Calculate the osmotic pressure of 0.03 mole of non electrolyte solute dissolved in $0.1 \mathrm{dm}^3$ of water at $300 \mathrm{~K} .\left[\mathrm{R}=0.082 \mathrm{dm}^3 \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right]$

Calculate the concentration of dissolved gas in water at $25^{\circ} \mathrm{C}$ if partial pressure of gas at same temperature is 0.15 atm .
\(\left[\mathrm{K}_{\mathrm{H}}=0.15 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~atm}^{-1}\right]\)

Which of the following solutions exhibits highest freezing point depression?

Calculate the molality of nonvolatile solution if solution freezes at $-0.95^{\circ} \mathrm{C}$
$\left[K_f\right.$ for water, $=1.86 \mathrm{~K} \mathrm{~mol}^{-1}$, freezing point of water $=0^{\circ} \mathrm{C}$ ]

Find the expected value of $\Delta \mathrm{T}_{\mathrm{b}}$ for $1 \mathrm{~m} \mathrm{AlCl}{ }_3$ solution in water if solution of nonelectrolyte of same concentration has $\Delta \mathrm{T}_{\mathrm{b}}$ value ' $x$ ' K .

Calculate vapour pressure of pure volatile liquid $B$ at given temperature if mole faction of liquid $B$ and vapour pressure of pure volatile liquid $A$ are 0.4 and 400 mm Hg respectively.
$$ \left[\mathrm{P}_{\text {total }}=600 \mathrm{~m...

Find molar mass of nonvolatile solute when 20 g of it dissolved in 200 g water at 300 K . [Relative lowering of vapour pressure $=0.02$ ]

Calculate the percent dissociation of 0.02 m solution if its freezing point depression is 0.046 K .
$\left[\mathrm{K}_{\mathrm{f}}\right.$ for water $\left.=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} ; \mathrm{n}=2\right]$

Which from following mixtures obeys Raoult's law?

Calculate the molal elevation constant of solvent if boiling point of 0.12 m solution is 319.8 K (Boling point of solvent $=319.5 \mathrm{~K}$ )

Calculate the concentration of an aqueous solution of non electrolyte at 300 K if its osmotic pressure is 12 atm .
\(\left[\mathrm{R}=0.0821 \mathrm{~atm} \mathrm{dm}^3 \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]\)

Identify from following salts so that the solubility of salt in water decreases with increase in temperature.

Which from following compounds is least soluble in water at STP?

What is the osmotic pressure of solution prepared by dissolving 3 gram solute in $2 \mathrm{dm}^3$ water at 300 K .
(Molar mass of solute $=60 \mathrm{~g} \mathrm{~mol}^{-1}$, $\mathrm{R}=0.0821 \mathrm{dm}^3 \mathrm{~atm} \mathrm{~K} \math...

Calculate the cryoscopic constant of solvent when 2.5 gram solute is dissolved in 35 gram solvent lowers its freezing point by 3 K. (molar mass of solute is $117 \mathrm{~g} \mathrm{~mol}^{-1}$)

Identify the reason for the solubility of polar solute in polar solvent from the following.

Assuming complete ionisation, arrange the following solutions in order of increasing osmotic pressure.
a) $0.5 \mathrm{~m} \mathrm{~Li}_2 \mathrm{SO}_4$
b) $\mathrm{0.5 ~m~KCl}$
c) $0.5 \mathrm{~m} \mathrm{~Al}_2\left(\mathrm{SO}_4\right)_3...

A solution of non volatile solute has boiling point elevation 0.5 K . Calculate molality of solution $\left[\mathrm{K}_{\mathrm{b}}=2.40 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$.

Calculate the molar mass of solute in a solution prepared by dissolving 1 gram in $0.3 \mathrm{~dm}^3$ solvent having osmotic pressure 0.2 atm at 300 K.
$$\left[\mathrm{R}=0.082 \mathrm{~dm}^3 \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-...

Calculate the molar mass of non volatile solute when 1 g of it is dissolved in 100 g solvent decreases its freezing point by 0.2 K .
$\left[\mathrm{K}_{\mathrm{f}}=1.2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

Calculate vapour pressure of a solution containing mixture of 2 moles of volatile liquid A and 3 moles of volatile liquid $B$ at room temperature. $\left(\mathrm{P}_{\mathrm{A}}^{\circ}=420, \mathrm{P}_{\mathrm{B}}^{\circ}=610 \mathrm{~mm} ...