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 –6°C will be: (Kf for water = 1.86 K kg mol–1 and molar mass of ethylene glycol = 62 g mol–1)
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By dissolving 5 g substance in 50 g of water, the decrease in freezing point is 1.2°C. The molal depression is 1.85°C. The molecular weight of substance is |
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The density (in g mL–1) of a 3.60 M sulphuric acid solution that is 29% H2SO4 (molar mass = 98 g mol–1) by mass will be |
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Dissolving 120 g of urea (mol. wt. 60) in 1000 g of water gave a solution of density 1.15 g/mL. The molarity of the solution is |
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A solution of two liquids boils at a temperature more than the boiling point of either of them. Hence, the binary solution shows ______. |
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The molality of a urea solution in which 0.0100 g of urea, [(NH2)2CO] is added to 0.3000 dm3 of water at STP is |
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A mixture of ethyl alcohol and propyl alcohol has vapour pressure of 290 mm at 300 K. The vapour pressure of propyl alcohol is 200 mm. If the mole fraction of ethyl alcohol is 0.6, its vapour pressure (in mm) at the same temperature will be |
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Molarity of 0.2 N H2SO4 is |
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A solution has 1 : 4 mole ratio of pentane to hexane. The vapour pressure of pure hydrocarbons at 20°C are 400 mm Hg for pentane and 120 mm Hg for hexane. The mole fraction of pentane in the vapour phase would be |
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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, then the above solution will freeze at |
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At 100ºC the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If Kb = 0.52, the boiling point of this solution will be: |
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