Chemistry Question Bank

Assertion: If red blood cells were removed from the body and placed in pure water, pressure inside the cells increases. Reason: The concentration of salt content in the cells increases.

Which observation(s) reflect(s) colligative properties? (i) A 0.5 m NaBr solution has a higher vapour pressure than a 0.5 m BaCl₂ solution at the same temperature (ii) Pure water freezes at the higher temperature than…

Assertion: The water pouch of instant cold pack for treating athletic injuries breaks when squeezed and NH₄NO₃ dissolves lowering the temperature. Reason: Addition of non-volatile solute into solvent results into depr…

Calculate the molarity of H₂SO₄ solution if the normality of H₂SO₄ Solution is 0.4 N.

At a particular temperature, the vapour pressures of two liquids A and B are respectively 120 and 180 mm of Hg respectively. If 2 moles of A and 3 moles of B are mixed to form an ideal solution, the vapour pressure of…

Calculate the molarity of Na₂CO₃ solution if the normality of Na₂CO₃ Solution is 0.2 N.

Vapour pessure of CCl₄ at 25ºC is 143 mm Hg. 0.5g of a non-volatile solute (mol. wt. 65) is dissolved in 100 cm3 of CCl₄. Find the vapour pressure of the solution. (Density of CCl₄ = 1.58 g/cm3).

The normality of 10% H₂SO₄ solution (d = 1.1g/cm3) is

25 mg of CaCO₃ is dissolved in 5 L of solution. The approximate concentration of solution is

The vapour pressure of solution of 5g of non- electrolyte in 100g of water at a particular temperature is 2985 Nm-2. The vapour pressure of pure water at that temperature is 3000 Nm-2. The molecular weight of the solu…

b b o cal C kg mol gm K K x x x

A 5% solution (by mass) of cane sugar in water has freezing point of 271 K and freezing point of pure water is 273.15 K. The freezing point of a 5% solution (by mass) of glucose in water is

The vapour pressure of a solvent decreases by 10 mm of Hg 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…

Exactly 1 g of urea dissolved in 75 g of water gives a solution that boils at 100.114°C at 760 torr. The molecular weight of urea is 60.1. The boiling point elevation constant for water is

When acetone and chloroform are mixed together, hydrogen bonds are formed between them. Which of the following statements is correct about the solution made by mixing acetone and chloroform?

12g of urea is dissolved in 1 litre of water and 68.4 g of sucrose is dissolved in 1 litre of water. The lowering of vapour pressure of first case is

A solution containing 10g per dm3 of urea(molecular mass = 60 g mol–1) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non- volatile solute is

A solution of urea (mol. mass 56 g mol-1) boils at 100.18 °C at the atmospheric pressure. If Kf and Kb for water are 1.86 and 0.512 K kg mol-1 respectively, the above solution will freeze at

A solution containing 1.8 g of a compound (empirical formula CH₂O) in 40 g of water is observed to freeze at –0.465 °C. The molecular formula of the compound is (Kf of water = 1.86 kg K mol–1)

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

An aqueous solution of NaCl shows the depression of freezing point of water equal to 0.372 K. The boiling point of BaCl₂ solution of same molality will be [Kf (H₂O)= 1.86 K kg mol–1; Kb(H₂O) = 0.52 K kg mol–1]

The freezing point of equimolal aqueous solution will be highest for

Assertion: Molecular mass of benzoic acid when determined by colligative properties is found high. Reason: Dimerisation of benzoic acid.

Assertion: The molecular weight of acetic acid determined by depression in freezing point method in benzene and water was found to be different. Reason: Water is polar, and benzene is nonpolar.

The latent heat of vaporisation of water is 9700 cal/mole and if the b.p. is 100 °C, the ebullioscopic constant of water is