Liquid Solution

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 ...

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 \(=0.346 \mathrm{~bar}]\)

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

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{~mo...

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} \mathr...

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

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

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

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

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

Which among the following solutions has minimum boiling point elevation?

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

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 \([0.159 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~bar}^{-1}]\) ?

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

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

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

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:

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} \mat...

Identify the FALSE statement about ideal solution from following.

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{~...

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

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{~...

What type of solution is the ethyl alcohol in water?

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}^{-...

What is the solubility of a gas in water at \(25^{\circ} \mathrm{C}\) if partial pressure is \(0.18 \mathrm{~atm}\) ? \(\left(\mathrm{K}_{\mathrm{H}}=0.16 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~atm}^{-1}\right)\)

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.

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} \m...

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.

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

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 ...

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

Air is an example of a solution of

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 \(=0^{\circ} \mathrm{C})\)

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...

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

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

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\(^{-1}\))

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

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)

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

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?

Which of the following formulae is used to obtain depression in freezing point?

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 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)

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

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?

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