Chemistry Question Bank

The freezing point of equimolal aqueous solutions will be highest for

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water fT , when 0.01 mole of sodium sulphate is dissolved in 1 kg of water, is…

Which of the following pair of solutions are expected to be isotonic at the same temperature?

Solutions A, B, C and D are respectively 0.1M glucose, 0.05 M NaCl, 0.05 M BaCl₂ and 0.1 M AlCl₃. Which one of the following pairs is isotonic?

The empirical formula of a non-electrolyte is CH₂O. A solution containing 6g/L of the compound exerts the same osmotic pressure as that of 0.05 M glucose solution. The molecular formula of the compound is SOLUTIONS

Van’t Hoff factor more than unity indicates that the solute in solution has

Two solutions A and B are separated by a semi- permeable membrane. As a result of osmosis, the level of solution A is found to rise. It implies that

Which of the following pairs of solutions is isotonic?

What would happen if a thin slice of sugar beet is placed in a concentrated solution of NaCl?

The Van’t Hoff factors i for an electrolyte which undergoes dissociation and association in solvents are respectively

Which of the following aqueous solutions has the highest boiling point?

0.1 M NaCl and 0.05 M BaC₁₂ solutions are separated by a semipermeable membrane in a container. For this system, choose the correct answer. (AMU 2010)

Kf for water is 1.86 K kg mol–1. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol (C₂H₆O₂) must you add to get the freezing point of the solution lowered to –2.8ºC?

The freezing point of 1 molal Glucose solution in water is ( 1.86 H O f K K kg mol )

Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at – 6ºC will be (Kf for water = 1.86 K kg mol–1. and molar mass o…

An aqueous solution of a non-electrolyte solute boils at 100.52ºC. The freezing point of the solution will be (Kf = 1.86K Kg mol-1, Kb = 0.52 K kg mol-1)

If 15 gm of a solute in 100 gm of water makes a solution that freezes at –1.0ºC, then 30 gm of the same solute in 100 gm of water will make a solution that freezes at

0.052 100.052 6 / 60 x x x x b b b b b o b T T T T T T C 102. An aqueous solution of Glucose freezes at –0.186 °C. Given that 0.512 H O b K K kg mol and 1.86 H O f K K kg mol , the elevation in boiling point of this s…

A solution of urea (mol. mass 56 g mol–1) boils at 100.18ºC 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

What weight of glycerol should be added to 600 g of water in order to lower its freezing point by 10ºC? (Kf = 1.86ºC m–1). (Molecular mass of glycerol is 92)

Depression of freezing point for …(i)… is directly proportional to …(ii)… Here, (i) and (ii) refer to

The amount of urea to be dissolved in 500 cc of water (K = 1.86) to produce a depression of 0.186ºC in the freezing point is

The freezing point of a 0.05 molal solution of a non- electrolyte in water is

Given that Tf is the depression in freezing point of the solvent in a solution of a nonvolatile solute of molality 1, the quantity f m T lt m → is equal to

Pure benzene freezes at 5.45ºC at a certain place but a 0.374m solution of tetrachloroethane in benzene freezes at 3.55ºC. The Kf for benzene is