Two liquids X and Y form an ideal solution. At 300 K, vapour pressure of the solution containing 1 mole of X and 3 mole of Y is 550 mm Hg. At the same temperature, if 1 mole of Y is further added to this solution, vapour pressure (in mm Hg) ofX and Y in their pure states will be respectively
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The vapour pressure of water at 23°C is 19.8 mm. 0.1 mole of glucose is dissolved in 178.2 g of water. What is the vapour pressure (in mm) of the resultant solution? |
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Equal volumes of 0.1 M and 0.2 M NaCl solutions are mixed. The concentration of nitrate ions in the resultant mixture will be |
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The elevation in boiling point of a solution of 13.44 g of CuCl2 in 1 kg of water using following information will be (molecular wt. of CuCl2 = 134.4, Kb = 0.52 K molal–1) |
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The freezing point (in °C) of a solution containing 0.1 g of K3[Fe(CN)6] (Mol. Wt. 329) in 100 g water (Kf = 1.86 K kg mol–1) is |
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25 mL of a solution of barium hydroxide on titration with 0.1 molar solution of hydrochloric acid gave a titre value of 35 mL. The molarity of barium hydroxide solution was |
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2 N HCl solution will have same molar concentration as a |
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An aqueous solution of glucose is 20% in strength. The volume in which 1 g mole of it is dissolved will be |
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10 cm3 of 0.1 N monobasic acid requires 15 cm3 of sodium hydroxide solution whose normality is |
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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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