Solutions Test ...

Determine the molarity of \(30 {~g}\) of \({CO}({NO})_{3} .6 {H}_{2} {O}\) in \(4.3 {~L}\) of solution.

To lower the melting point of \(75 {~g}\) of acetic acid by \(1.5^{\circ} {C}\), how much mass of ascorbic acid is needed to be dissolved in the solution where \(K_{f}=3.9\) \({K} {~kg} {~mol}^{-1}\)?

Which one of the following is a primary standard?

At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration?

An aqueous solution of hydrochloric acid:

A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the solvent in resulting solution.

100 g of liquid A (molar mass 140 g mol^–1) was dissolved in 1000 g of liquid B (molar mass 180 g mol–1). The vapour pressure of pure liquid B was found to be 500 torrs. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 Torr.

If \(1.202 {~g} {~mL}^{-1}\) is the density of \(20 \%\) aqueous KI, determine the molality of KI.

\(12 {~g}\) of urea is present in 1 litre of solution and \(68.4 {~g}\) of sucrose is separately dissolved in 1 litre of another sample of solution. The lowering of vapour pressure of first solution is:

In an endothermic process, solubility increases with ______ in temperature.

During osmosis, flow of water through a semi-permeable membrane is:

A solution of acetone in ethanol:

A student slowly mixes salt into 25 ml of water until no more salt dissolves in it. The student could make more salt dissolve in the solution by:

Calculate the mass of ascorbic acid ( \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\) ) to be dissolved in \(75 \mathrm{~g}\) of acetic acid to lower its melting point by \(1.5^{\circ} \mathrm{C}\). Take \( \mathrm{K}_{\mathrm{f}}=3.9 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\).

Which of the following 0.10m aqueous solution will have the lowest freezing point?

Exactly \(1 {~g}\) of urea dissolved in \(75 {~g}\) of water gives a solution that boils at \(100.114^{\circ} {C}\) at 760 torr. The molecular weight of urea is \(60.1\). The boiling point elevation constant for water is:

The vapour pressure of a solvent decreased by 10 mm of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent, if the decrease in the vapour pressure is to be 20 mm of mercury?

\(1.00 {~g}\) of a non- electrolyte solute (molar mass \(250 {~g} {~mol}^{-1}\) ) was dissolved in \(51.2 {~g}\) of benzene. If the freezing point depression constant, \({K}_{{f}}\) of benzene is \(5.12 {~k} {~kg} {mol}^{-1}\), the freezing point of benzene will be lowered by:

If benzene in solution containing 30% by mass in carbon tetrachloride, calculate the mole fraction of benzene.

How much of sucrose is to be added to 500 g of water such that it boils at 100°C if the molar elevation constant for water is 0.52 K kg mol^-1 and the boiling point of water at 750 mm Hg is 99.63°C?

Heptane and octane form an ideal solution. At 373 K, the vapour pressures of the two liquid components are 105.2 kPa and 46.8 kPa respectively. What will be the vapour pressure of a mixture of 26.0 g of heptane and 35 g of octane?

Which of the following pair will form an ideal solution?

At a particular temperature, the vapour pressures of two liquids A and B are 120 mm and 180 mm of mercury respectively. If 2 moles of A and 3 moles of B are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be: (in mm of mercury)

If a solution prepared by dissolving 1.0 g of polymer of molar mass 185,000 in 450 mL of water at 37°C, calculate the osmotic pressure in Pascal exerted by it?

A solution containing \(10 {~g}\) per \({dm}^{3}\) of urea (molecular mass \(\left.=60 {~g} {~mol}^{-1}\right)\) is isotonic with a \(5 \%\) solution of a non-volatile solute. The molecular mass of this non-volatile solute is:

A solution containing \(1.8 {~g}\) of a compound (empirical formula \({CH}_{2} {O}\) ) in \(40 {~g}\) of water is observed to freeze at \(-0.465 {C}\). The molecular formula of the compound is \(({K_f}\) of water \(=1.86 {~kg}\) \(\left.{kmol}^{-1}\right)\)

An aqueous solution of 2% non-volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molar mass of the solute?

The freezing point of equimolal aqueous solution will be highest for:

If \(22 {~g}\) of benzene is dissolved in \(122 {~g}\) of carbon tetrachloride, determine the mass percentage of carbon tetrachloride \(\left({CCl}_{4}\right)\) and benzene \(\left({C}_{6} {H}_{6}\right)\).

Calculate the amount of benzoic acid \(\left({C}_{6} {H}_{5} {COOH}\right)\) required for preparing 250 \({mL}\) of \(0.15 {M}\) solution in methanol.