Chemistry Question Bank

Which statement is incorrect about osmotic pressure (), volume (V) and temperature (T)?

During freezing of a solution the following are in equilibrium

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…

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

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?

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

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

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…

Raoult's law states that for a dilute solution,

What happens to freezing point of benzene when naphthalene is added?

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

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

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)

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

An aqueous solution freezes at –2.550C. What is its boiling point. 0.52 / ; 1.86 / ? H O H O b f K K m K K m

Sprinkling of salt helps in clearing the snow covered roads in hills. The phenomenon involved in the process 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

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 molal b.p. constant for water is 0.5130C kg mol– 1. When 0.1 mole of sugar is dissolved in 200 g of water, the solution boils under a pressure of 1 atm at

If the elevation in boiling point of a solution of 10gm of solute (mol. wt. = 100) in 100 gm of water is bT , then ebullioscopic constant of water is

Elevation in boiling point was 0.520C when 6 gm of a compound X was dissolved in 100 gm of water. Molecular weight of X is (Kb of water is 0.52 K⁻ kg/mol)

The molar freezing point constant for water is 1.86º C/m. If 342g of cane sugar (C₁₂H₂₂O₁₁) is dissolved in 1000 g of water, the solution will freeze at

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

Colligative properties of the solution depend on