19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
The Van’t Hoff factors i for an electrolyte which undergoes dissociation and association in solvents are respectively
Van’t Hoff factor more than unity indicates that the solute in solution has
The freezing point of equimolal aqueous solutions will be highest for
In which mode of expression, the concentration of solution remains independent of temperature?
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
What would happen if a thin slice of sugar beet is placed in a concentrated solution of NaCl?
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?
Among 0.1 M solutions of urea, Na₃PO₄ and Al₂ (SO₄)₃, which is incorrect
Which statement is incorrect about osmotic pressure (), volume (V) and temperature (T)?
Which of the following colligative properties can provide molar mass of proteins (or polymers of colloids) with greater precision?
Which of the following pairs of solutions is isotonic?
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…
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
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
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…
An aqueous solution is 1.0 molal in KI. Which change will cause the vapour pressure of the solution to increase? (AIPMT 2010)
If liquid A and B from ideal solutions
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 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
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
Depression of freezing point for …(i)… is directly proportional to …(ii)… Here, (i) and (ii) refer 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
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)
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)
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