Liquid Solution · Chemistry · MHT CET

What type of solution is the iodine in air?

Calculate the relative lowering of vapour pressure if vapour pressure of pure solvent and vapour pressure of solution at $25^{\circ} \mathrm{C}$ are 32 and 30 mm Hg respectively.

Calculate the molality of solution if its depression in freezing point is 0.18 K . $\left[\mathrm{K}_{\mathrm{f}}=1.6 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

Identify the correct statement from following properties.

Calculate van't Hoff factor of 0.15 M solution of electrolyte if it freezes at $-$0.5 K.

$$\left[\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$$

Calculate the relative lowering of vapour pressure of solution containing 46 g of non volatile solute in 162 g of water at $20^{\circ} \mathrm{C}$. [Molar mass of nonvolatile solute $=46 \mathrm{~g} \mathrm{~mol}^{-1}$]

Calculate molar mass of a solute at 300 K if 400 mg of it is dissolved in 300 mL of water exerts osmotic pressure of 0.2 atm .

$$\left(\mathrm{R}=0.0821 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$$

What is the vapour pressure of a solution containing 0.1 mol of non volatile solute dissolved in 16.2 g water? $\left(\mathrm{P}_1^0=24 \mathrm{mmHg}\right.$, molar mass of water $18 \mathrm{~g} \mathrm{~mol}^{-1}$ )

What is the expected value of $\Delta T_f$ for $1.25 \mathrm{~m} \mathrm{CaCl}_2$ solution if 1.25 m sucrose solution has $\Delta \mathrm{T}_{\mathrm{f}}$ value x K ?

Calculate Henry's law constant if solubility of gas in water at $25^{\circ} \mathrm{C}$ is $5.14 \times 10^{-4} \mathrm{~mol} \mathrm{dm}^{-3}$ and partial pressure of the gas is 0.75 bar above solution.

A solution of nonvolatile solute is obtained by dissolving 0.8 g in $0.3 \mathrm{dm}^3$ water has osmotic pressure 0.2 atm at 300 K . Calculate the molar mass of solute.

$$\left[\mathrm{R}=0.082 \mathrm{~atm} \mathrm{dm}^3 \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$$

In a solution, mole fraction of solute is 0.2 , when lowering in vapour pressure is 10 mm Hg . To get lowering of vapour pressure of 20 mm Hg , mole fraction of solute in solution is

Which of the following solutions will not show flow of solvent in either direction when separated by semipermeable membrane?

The solution containing $18 \mathrm{~g} \mathrm{dm}^{-3}$ glucose (molar mass 180) in water and another containing $6 \mathrm{~g} \mathrm{dm}^{-3}$ of solute A in water boils at same temperature. What is molar mass of A ?

If $P_1$ partial pressure of a gas and $x_1$ is its mole fraction in a mixture, then correct relation between $P_1$ and $x_1$ is

Calculate van't Hoff factor (i) of 0.2 m aqueous solution of an electrolyte if it freezes at $-0.660 \mathrm{~K} .\left(\mathrm{K}_{\mathrm{f}}=1.84 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

Vapour pressure of a pure solvent is 550 mm of Hg . By addition of a non volatile solute it decreases to 510 mm of Hg . Calculate the mole fraction of solute in solution.

Identify the false statement among the following.

Calculate the solubility of a gas having partial pressure 0.15 bar at $25^{\circ} \mathrm{C}$. $\left[\mathrm{K}_{\mathrm{H}}=0.16 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{bar}^{-1}\right]$

Which from following ionic solids exhibits decrease in its solubility in water with increase of temperature?

Calculate molar mass of nonvolatile solute if a solution containing 0.35 g solute in 100 g water has boiling point elevation 0.01 K $\left[\mathrm{K}_{\mathrm{b}}=0.50 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right.$ ]

0.2 molal aqueous solution of KCl freezes at $-0.680^{\circ} \mathrm{C}$. Calculate van't Hoff factor for this solution. $\left(\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

0.1 molal aqueous solution of glucose boils at $100.16^{\circ} \mathrm{C}$. What is boiling point of 0.5 molal aqueous solution of glucose?

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.

$$\left[\mathrm{R}=0.082 \mathrm{~dm}^3 \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$$

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) $0.5 \mathrm{~m} \mathrm{~Al}_2\left(\mathrm{SO}_4\right)_3$

d) $0.1 \mathrm{~m~BaCl}_2$

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.

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 $=60 \mathrm{~g} \mathrm{~mol}^{-1}$, $\mathrm{R}=0.0821 \mathrm{dm}^3 \mathrm{~atm} \mathrm{~K} \mathrm{~mol}^{-1})$

Calculate the molar mass of solute when 4 g of it dissolved in $1 \mathrm{dm}^3$ solvent has osmotic pressure 2 atm at 300 K . [R $\left[=0.082 \mathrm{~dm}^3 \mathrm{~atm} \mathrm{~K} \mathrm{~mol}^{-1}\right]$

Calculate $\Delta \mathrm{T}_{\mathrm{f}}$ of aqueous 0.01 m formic acid if van't Hoff factor is 1.1

$$\left[\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~Kg} \mathrm{~mol}^{-1}\right]$$

What is the relation between the vapour pressure of solution, vapour pressure of solvent and its mole fraction in the solution?

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. $\left(\mathrm{P}_{\mathrm{A}}^{\circ}=420, \mathrm{P}_{\mathrm{B}}^{\circ}=610 \mathrm{~mm} \mathrm{~Hg}\right.$)

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 . $\left[\mathrm{K}_{\mathrm{f}}=1.2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

Which of the following solutions on complete dissociation exhibits maximum elevation in boiling point?

The molal elevation boiling point constant for water is $0.513^{\circ} \mathrm{C} \mathrm{Kg} \mathrm{mol}^{-1}$. Calculate boiling point of solution if 0.1 mole of sugar is dissolved in 200 g water?

What mass of solute (molar mass $58 \mathrm{~g} \mathrm{~mol}^{-1}$) is to be dissolved in $2.5 \mathrm{~dm}^3 \mathrm{~H}_2 \mathrm{O}$ to generate osmotic pressure of 0.245 atm at 300 K ?

$$\left(\mathrm{R}=0.0821 \mathrm{~dm}^3 \text { atm } \mathrm{K}^{-1} \mathrm{~mol}^{-1}\right)$$

Which of the following equation correctly represents molar mass of a solute by knowing boiling point elevation?

A solution of non volatile solute has boiling point elevation 1.75 K . Calculate molality of solution $\left[\mathrm{K}_{\mathrm{b}}=3.5 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

Which from the following statements is correct for aqueous solution of $6 \mathrm{~g} \mathrm{~L}^{-1}$ urea and $17 \cdot 12 \mathrm{~g} \mathrm{~L}^{-1}$ of sucrose?

[Molar mass of urea $=60 \mathrm{~g} \mathrm{~mol}^{-1}$

Molar mass of sucrose $=342 \mathrm{~g} \mathrm{~mol}^{-1}$]

Calculate the molar mass of nonvolatile solute when 1.5 g of it is dissolved in 90 g solvent decreases its freezing point by 0.25 K. $$\left[\mathrm{K}_{\mathrm{f}}=1.2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$$

Identify false statement form following.

Calculate van't Hoff factor of 0.2 m aquesous solution of an electrolyte if it freezes at $-$0.7 K $\left[\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

Calculate the molar mass of non volatile solute when 5 g of it is dissolved in 50 g solvent, boils at $119.6^{\circ} \mathrm{C}$. $\left[\mathrm{K}_{\mathrm{b}}=3.2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right.$, boiling point of pure solvent $=118^{\circ} \mathrm{C}$ ].

Identify an example of solution that consists of solid as solute and liquid as solvent.

Calculate the molality of solution of non volatile solute having depression in freezing point 0.93 K and cryoscopic constant of solvent $1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$.

A solution of non volatile solute is obtained by dissolving 2 g in 50 g benzene. Calculate the vapour pressure of solution if vapour pressure of pure benzene is 640 mmHg at $25^{\circ} \mathrm{C}$. [mol. mass of benzene $=78 \mathrm{~g} \mathrm{~mol}^{-1}$, mol. mass of solute $\left.=64 \mathrm{~g} \mathrm{~mol}^{-1}\right]$

What is Henry's law constant of a gas if solubility of gas in water at $$25^{\circ} \mathrm{C}$$ is $$0.028 \mathrm{~mol} \mathrm{~dm}^{-3}$$ ?

[Partial pressure of gas $$=0.346 \mathrm{~bar}]$$

A solution of nonvolatile solute is obtained by dissolving $$15 \mathrm{~g}$$ in $$200 \mathrm{~mL}$$ water has depression in freezing point $$0.75 \mathrm{~K}$$. Calculate the molar mass of solute if cryoscopic constant of water is $$1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$.

What type of following solutions is the gasoline?

Calculate the relative lowering of vapour pressure if the vapour pressure of benzene and vapour pressure of solution of non-volatile solute in benzene are $$640 \mathrm{~mmHg}$$ and $$590 \mathrm{~mmHg}$$ respectively at same temperature.

Calculate the depression in freezing point of solution when $$4 \mathrm{~g}$$ nonvolatile solute of molar mass $$126 \mathrm{~g} \mathrm{~mol}^{-1}$$ dissolved in $$80 \mathrm{~mL}$$ water [Cryoscopic constant of water $$=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$ ]

Which among the following is NOT colligative property?

What is the molality of solution of a non-volatile solute having boiling point elevation $$7.15 \mathrm{~K}$$ and molal elevation constant $$2.75 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$ ?

Which among the following salts exhibits inverse relation between it's solubility and temperature?

If $$0.01 \mathrm{~m}$$ aqueous solution of an electrolyte freezes at $$-0.056 \mathrm{~K}$$. Calculate van't Hoff factor for an electrolyte (cryoscopic constant of water $$=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$ )

Calculate van't Hoff factor of $$\mathrm{K}_2 \mathrm{SO}_4$$ if $$0.1 \mathrm{~m}$$ aqueous solution of $$\mathrm{K}_2 \mathrm{SO}_4$$ freezes at $$-0.43{ }^{\circ} \mathrm{C}$$ and cryoscopic constant of water is $$1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$.

A solution of $$5.6 \mathrm{~g}$$ non-volatile solute in $$50 \mathrm{~g}$$ solvent has elevation in boiling point $$1.75 \mathrm{~K}$$. What is the molar mass of solute $$\left(\mathrm{K}_{\mathrm{b}}=3 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$$ ?

What is the molal elevation constant if one gram mole of a nonvolatile solute is dissolved in $$1 \mathrm{~kg}$$ of ethyl acetate? $$\left(\Delta \mathrm{T}_{\mathrm{b}}=x \mathrm{~K}\right)$$

If $$0.15 \mathrm{~m}$$ aqueous solution of KCI freezes at $$-0.511^{\circ} \mathrm{C}$$, calculate van't Hoff factor of KCI (cryoscopic constant of water is $$1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1})$$

What is the solubility of gas in water at $$25^{\circ} \mathrm{C}$$ if partial pressure is 0.346 bar [Henry's law constant is $$[0.159 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~bar}^{-1}]$$ ?

The partial vapour pressure of any volatile component of a solution is equal to the vapour pressure of the pure component multiplied by its mole fraction in the solution is called

Which among the following solutions has minimum boiling point elevation?

Calculate osmotic pressure of solution of 0.025 mole glucose in $$100 \mathrm{~mL}$$ water at $$300 \mathrm{~K}$$. $$\left[\mathrm{R}=0.082 \mathrm{~atm} \mathrm{dm} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right]$$

Calculate molality of solution of a nonvolatile solute having boiling point elevation $$1.89 \mathrm{~K}$$ if boiling point elevation constant of solvent is $$3.15 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$.

A solution of nonvolatile solute is obtained by dissolving $$1.5 \mathrm{~g}$$ in $$30 \mathrm{~g}$$ solvent has boiling point elevation $$0.65 \mathrm{~K}$$. Calculate the molal elevation constant if molar mass of solute is $$150 \mathrm{~g} \mathrm{~mol}^{-1}$$.

Identify the FALSE statement about ideal solution from following.

Calculate osmotic pressure of $$0.2 \mathrm{~M}$$ aqueous $$\mathrm{KCl}$$ solution at $$0^{\circ} \mathrm{C}$$ if van't Hoff factor for $$\mathrm{KCl}$$ is 1.83. $$\left[\mathrm{R}=0.082 \mathrm{~dm}^3 \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right]$$

If $$\mathrm{K}_{\mathrm{b}}$$ denote molal elevation constant of water, then boiling point of an aqueous solution containing $$36 \mathrm{~g}$$ glucose (molar mass $$=180$$ ) per $$\mathrm{dm}^3$$ is:

What is vapour pressure of a solution containing $$1 \mathrm{~mol}$$ of a nonvolatile solute in $$36 \mathrm{~g}$$ of water $$\left(\mathrm{P}_1^0=32 \mathrm{~mm} \mathrm{~Hg}\right)$$ ?

Which among following salts shows decrease in solubility with increase in temperature?

The solubility of a gas in a liquid is directly proportional to the pressure of the gas over the solution. Identify the law for this statement.

What is the solubility of a gas in water at $$25^{\circ} \mathrm{C}$$ if partial pressure is $$0.18 \mathrm{~atm}$$ ?

$$\left(\mathrm{K}_{\mathrm{H}}=0.16 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~atm}^{-1}\right)$$

What is osmotic pressure of solution of $$1.7 \mathrm{~g} \mathrm{~CaCl}_2$$ in $$1.25 \mathrm{~dm}^3$$ water at $$300 \mathrm{~K}$$ if van't Hoff factor and molar mass of $$\mathrm{CaCl}_2$$, are 2.47 and $$111 \mathrm{~g} \mathrm{~mol}^{-1}$$ respectively?

$$\left[\mathrm{R}=0.082 \mathrm{~dm}^3 \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right]$$

What type of solution is the ethyl alcohol in water?

Find the depression in freezing point of solution when 3.2 gram non volatile solute with molar mass $$128 \mathrm{~gram} \mathrm{~mol}^{-1}$$ is dissolved in $$80 \mathrm{~gram}$$ solvent if cryoscopic constant of solvent is $$4.8 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$.

Which of the following solutions exhibits lowest value of boiling point elevation assuming complete dissociation?

A solution of $$8 \mathrm{~g}$$ of certain organic compound in $$2 ~\mathrm{dm}^3$$ water develops osmotic pressure $$0.6 \mathrm{~atm}$$ at $$300 \mathrm{~K}$$. Calculate the molar mass of compound. [R = 0.082 atm dm$$^3$$ K$$^{-1}$$ mol$$^{-1}$$]

Which from the following compound solutions in water of equal concentration has electrical conductivity nearly same as distilled water?

A solution of nonvolatile solute is obtained by dissolving $$1 \mathrm{~g}$$ in $$100 \mathrm{~g}$$ solvent, decreases its freezing point by $$0.3 \mathrm{~K}$$. Calculate cryoscopic constant of solvent if molar mass of solute is $$60 \mathrm{~g} \mathrm{~mol}^{-1}$$.

Which among the following gases exhibits very low solubility in water at room temperature?

$$0.2 ~\mathrm{M}$$ aqueous solution of glucose has osmotic pressure 4.9 atm at $$300 \mathrm{~K}$$. What is the concentration of glucose if it has osmotic pressure $$1.5 \mathrm{~atm}$$ at same temperature?

A solution of nonvolatile solute is obtained by dissolving $$3.5 \mathrm{~g}$$ in $$100 \mathrm{~g}$$ solvent has boiling point elevation $$0.35 \mathrm{~K}$$. Calculate the molar mass of solute.

(Molal elevation constant $$=2.5 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$ )

Calculate the solubility of a gas in water at $$0.8 \mathrm{~atm}$$ and $$25^{\circ} \mathrm{C}$$.

[Henry's law constant is $$6.85 \times 10^{-4} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~atm}^{-1}$$ ]

Identify the concentration of the solution from following so that values of ,$$\Delta \mathrm{T}_{\mathrm{f}}$$ and $$\mathrm{K}_{\mathrm{f}}$$ are same.

Calculate the amount of solute dissolved in 160 gram solvent that boils at $$85^{\circ} \mathrm{C}$$, the molar mass of solute is $$120 \mathrm{~g} \mathrm{~mol}^{-1}$$. $$\left(\mathrm{K}_{\mathrm{b}}\right.$$ for solvent $$=2.7^{\circ} \mathrm{C} \mathrm{~kg} \mathrm{~mol}^{-1}$$ and boiling point of solvent $$=76^{\circ} \mathrm{C}$$)

The solution containing $$3 \mathrm{~g}$$ urea (molar mass 60 ) per $$\mathrm{dm}^3$$ of water and another solution containing $$4.5 \mathrm{~g}$$ of solute $$\mathrm{A}$$ per $$\mathrm{dm}^3$$ boils at same temperature, then what is molar mass of $$\mathrm{A}$$ ?

Vapour pressure of solution and of pure solvent are $$\mathrm{P}_1$$ and $$\mathrm{P}_1{ }^0$$ respectively. If $$\frac{P_1}{P_1^0}$$ is 0.15, find the mole fraction of solute.

According to Raoult's law mole fraction of solute in solution in given by formula

What is vapour pressure of solution containing 0.1 mole solute dissolved in $$1.8 \times 10^{-2} \mathrm{~kg} \mathrm{~H}_2 0$$ ? $$(\mathrm{P}_1^0=24 \mathrm{~mm} \mathrm{~Hg})$$

What is vapour pressure of a solution containing $$1 \mathrm{~mol}$$ of a non-volatile solute in $$36 \mathrm{~g}$$ of water? $$(\mathrm{P}_1^0=400 \mathrm{~mm} \mathrm{Hg}$$)

Which of the following solutions behaves nearly as an ideal solution?

The solution containing $$6 \mathrm{~g}$$ urea (molar mass 60 ) per $$\mathrm{dm}^3$$ of water and another solution containing $$9 \mathrm{~g}$$ of solute $$\mathrm{A}$$ per $$\mathrm{dm}^3$$ water freezes at same temperature. What is molar mass of $$\mathrm{A}$$ ?

What is vapour pressure of solution containing $$1.8 \mathrm{~g}$$ glucose in $$16.2 \mathrm{~g}$$ water?

($$\mathrm{P}_1^0=24 \mathrm{~mm} \mathrm{Hg}$$ and Molar mass of glucose $$=180 \mathrm{~g} \mathrm{~mol}^{-1}$$)

What is the freezing point of 1 molal aqueous solution of a non volatile solute?

($$\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1})$$ ($$\mathrm{T}_{\mathrm{f}}^0$$ for water $$=0^{\circ} \mathrm{C})$$

Air is an example of a solution of

5 g sucrose (molar mass = 342) is dissolved in 100 g of solvent, decreases the freezing point by 2.15 K. What is cryoscopic constant of solvent?

What is Henry's law constant if solubility of a gas in water at $$298 \mathrm{~K}$$ and 1 bar pressure is $$7\times10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$$ ?

The vapour pressure of a solvent decreases by 2.5 mm Hg by adding a solute. What is the mole fraction of solute? (Vapour pressure of pure solvent is 250 mm Hg)

Molal depression constant for a liquid is $$2.77^{\circ} \mathrm{C} ~\mathrm{kg} ~\mathrm{mol}^{-1}$$, in Kelvin scale it's value is

If 6 g of solute dissolved in 100 g of water lowers the freezing point by 0.93 K. What is molar mass of solute? (K$$_\mathrm{f}$$ = 1.86 K kg mol$$^{-1}$$)

What is vapour pressure of a solution when $$2 \mathrm{~mol}$$ of a non-volatile solute are dissolved in $$20 \mathrm{~mol}$$ of water? $$\left(\mathrm{P}_1^0=32 \mathrm{~mm} \mathrm{Hg}\right)$$

In which of the following salts, the solubility increases appreciably with increase in temperature?

What is the boiling point of 0.5 molal aqueous solution of sucrose if 0.1 molal aqueous solution of glucose boils at 100.16$$^\circ$$C?

Which of the following solutions shows positive deviation from Raoult's law?

What is vapour pressure of a solution containing 0.1 mol of non-volatile solute dissolved in 16.2 g of water ? (P$$_1^0=32$$ mm Hg)

What is boiling point of a decimolal aqueous solution of glucose if molal elevation constant for water is 0.52$$^\circ$$C kg mol$$^{-1}$$ ?

What is cryoscopic constant of water if $$5 \mathrm{~g}$$ of glucose in $$100 \mathrm{~g}$$ of water has depression in freezing point $$2.15 \mathrm{~K}$$ ? (Molar mass of glucose $$=180$$ )

Which of the following statements is correct for boiling point of a liquid?

Henry's law constant for $$\mathrm{CH}_3 \mathrm{Br}$$ is $$0.16 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{bar}^{-1}$$ at $$298 \mathrm{~K}$$. What pressure is required to have solubility of $$0.08 \mathrm{~mol} \mathrm{~L}^{-1}$$ ?

Which of the following solutions does not flow in either direction, when separated by semipermeable membrane? (Molar mass : glucose = 180, urea = 60)

A solution of 6 g of solute in 100 g of water boils at 100.52$$^\circ$$C. The molal elevation constant of water is 0.52 K kg mol$$^{-1}$$. What is molar mass of solute?

If vapour pressure of pure solvent and solution are 240 and 216 mm Hg respectively then mole fraction of solvent in solution is

The vapour pressure of solvent decreases by 10 mm Hg , if mole fraction of non-volatile solute is 0.2 . Calculate vapour pressure of solvent.

Which of the following $0-10 \mathrm{~m}$ aqueous solutions will have maximum $\Delta T_f$ value?

If boiling point of urea solution is $100.18^{\circ} \mathrm{C}$ and $K_b$ for water is $0.512 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$, molality of solution is (Boiling point of water $=100^{\circ} \mathrm{C}$)

What is osmotic pressure of a semi molar solution at $$27^{\circ} \mathrm{C}$$ ? $$(R=0.082)$$

Solutions $$A, B, C$$ and $$D$$ are respectively 0.2 M urea, $$0.10 \mathrm{~M} \mathrm{~NaCl}, 0.05 \mathrm{~M} \mathrm{~BaCl}_2$$ and 0.05 M $$\mathrm{AlCl}_3$$. All solutions are isotonic with each other except

A solution has an osmotic pressure of '$$x$$' $$\mathrm{kPa}$$ at $$300 \mathrm{~K}$$ having 1 mole of solute in $$10.5 \mathrm{~m}^3$$ of solution. If it's osmotic pressure is reduced to $$\left(\frac{1}{10}\right)$$th of it's initial value, what is the new volume of solution?

If a centimolal aqueous solution of K$$_3$$[Fe(CN)$$_6$$] has degree of dissociation 0.78. What is the value of van't Hoff factor?

The elevation in boiling point of 0.25 molal aqueous solution of a substance is $\left(K_o=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

Which among the following salts, solubility decreases with increase in temperature?

18 gram glucose (Molar mass $=180$ ) is dissolved in 100 ml of water at 300 K . If $R=3$ $0.0821 \mathrm{~L}{-\mathrm{a t m}} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ what is the osmotic pressure of solution?

Relationship between van't Hoff's factor (i) and degree of dissociation $(\alpha)$ is

9 gram anhydrous oxalic acid (mol. $\mathrm{wt} .=90)$ was dissolved in 9.9 moles of water. If vapour pressure of pure water is $p_1^{\circ}$ the vapour pressure of solution is

Which of the following sets of solutions of urea ( mol . mass $60 \mathrm{~g} \mathrm{~mol}^{-1}$ ) and sucrose ( mol . mass $342 \mathrm{~g} \mathrm{~mol}^{-1}$ ) is isotonic?

Which of the following sets of components form homogeneous mixture?

Calculate van't Hoff-factor for 0.2 m aqueous solution of KCl which freezes at $-0.680^{\circ} \mathrm{C}$. $\left(K_f=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

' $K$ is Henry's constant and has the unit