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question_answer1) Direction (1 - 20): The questions given below consist of Assertion and Reason. Use the following key to select the correct answer. Assertion: Molarity of a solution in liquid state changes with temperature. Reason: The volume of a solution changes with change in temperature.
question_answer2) Assertion: Solubility of gases in liquids increases with increase in pressure. Reason: Dissolution of gas in a liquid is exothermic in nature.
question_answer3) Assertion: When a solution is separated from the pure solvent by a semi-permeable membrane, the solvent molecules pass through it from pure solvent side to the solution side. Reason: Diffusion of solvent occurs from a region of high concentration solution to a region of low concentration solution.
question_answer4) Assertion: van't Hoff factor for benzoic acid is less than 1 in benzene. Reason: Benzoic acid associates in benzene.
question_answer5) Assertion: Ethyl alcohol and water form maximum boiling azeotrope. Reason: Attractive forces in solution tend to decrease.
question_answer6) Assertion: In an ideal solution, AH mixing is zero. Reason: A.......... B interactions are the same as A.......... A and B.......... B interactions.
question_answer7) Assertion: Out of various colligative properties, only osmotic pressure is used to determine the molecular masses of polymers. Reason: Polymer solutions donot possess a constant boiling point or freezing point.
question_answer8) Assertion: Cooking time is reduced in pressure cooker. Reason: Boiling point of water inside the pressure cooker is lowered.
question_answer9) Assertion: The molecular mass of acetic acid was determined by depression in freezing point method in benzene and was found to be different than in water. Reason: Water is polar and benzene is non-polar.
question_answer10) Assertion: The boiling point of \[0\centerdot 1M\] urea solution is less than \[0\centerdot 1M\] KCI solution. Reason: Elevation of boiling point is directly proportional to the number of species present in the solution.
question_answer11) Assertion: Aquatic species are more comfortable in warm water than in cold water. Reason: \[{{K}_{H}}\] values for both \[{{N}_{2}}\] and \[{{O}_{2}}\] increase with increase in temperature.
question_answer12) Assertion: When methyl alcohol is added to water, boiling point of water increases. Reason: Methyl alcohol and water forms minimum boiling azeotope.
question_answer13) Assertion: When NaCI is added to water, a depression in freezing point is observed. Reason: The lowering of vapour pressure of a solution causes depression in the freezing point.
question_answer14) Assertion: Molality is preferred to molarity for expressing the concentration of the solution. Reason: Molality can be determined more easily than molarity.
question_answer15) Assertion: Among equimolar solutions of KCI and \[{{K}_{2}}S{{O}_{4}}\], osmotic pressure is lower for KCI solution. Reason: \[{{K}_{2}}S{{O}_{4}}\] releases more ions in solution than KCI.
question_answer16) Assertion: If red blood cells were removed from the body and placed in pure water, the pressure inside the cells increases. Reason: The concentration of the salt content in the cells increases.
question_answer17) Assertion: The boiling point of \[0\centerdot 1M\] urea solution is less than \[0\centerdot 1M\] KCl solution. Reason: Elevation of boiling point is directly proportional to the number of species present in the solution.
question_answer18) Assertion: Aquatic species are more comfortable in cold water than in warm water. Reason: \[{{K}_{H}}\] values for both \[{{N}_{2}}\] and \[{{O}_{2}}\] decrease with increase in temperature.
question_answer19) Assertion: Acetone-aniline mixture shows nagative deviation from Raoult's law Reason: H-bonding between acetone and aniline is stronger than that between acetone-acetone and aniline-aniline.
question_answer20) Assertion: The vapour pressure of a liquid decreases if some non-volatile solute is dissolved in it. Reason: The relative lowering of vapour pressure of a solution containing a non-volatile solute is equal to the mole fraction of the solute in the solution.
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