19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
If boiling point of water is 1000C. How much gram of NaCl is added in 500 g of water to increase its boiling point by approx o b H O 1 C K 0.52K kg / mole. x (AllMS 2019)
The mixture which shows positive deviation from Raoult’s law is: (NEET 2020)
The freezing point depression constant f K of benzene is 5.12 K kg mol-1. The freezing point depression for the solution of molality 0.078 m containing a non- electrolyte solute in benzene is (rounded off upto two dec…
The following solutions were prepared by dissolving 10 g glucose (C₆H₁₂O₆) in 250 ml of water (P₁) 10 g of urea (CH₄N₂O) in 250 ml of water (P₂) and 10 g of sucrose (C₁₂H₁₂O₁₁) in 250 ml of water (P₃). The right optio…
The correct option for the value of vapour pressure of a solution at 45 °C with benzene to octane in molar ratio 3 : 2 is: [At 45 °C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume idea…
25 mg of CaCO₃ is dissolved in 5 L of solution. The approximate concentration of solution is
The normality of 10% H₂SO₄ solution (d = 1.1g/cm3) is
Calculate the molarity of Na₂CO₃ solution if the normality of Na₂CO₃ Solution is 0.2 N.
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…
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 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…
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
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)
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]
An aqueous solution of NaCl 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 solution is
The freezing point of equimolal aqueous solution will be highest for
Which of the following 0.10 m aqueous solutions will have the lowest freezing point?
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: If a liquid solute more volatile than the solvent is added to the solvent, the vapour pressure of the solution may increase. Reason: In the presence of a more volatile liquid solute, only the solute will fo…
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…
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.
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.
Assertion: Lowering of vapour pressure is directly proportional to osmotic pressure of the solution. Reason: Osmotic pressure is a colligative property.