Quiz 9 for Class 12 Chemistry Chapter 2 Solutions

Quiz 9 for Class 12 Chemistry Chapter 2 Solutions

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Quiz 9 : Solutions - Class 12 Chemistry

Negative Marking :- No

Weightage per Question :- 1 Mark

Number of Questions :- 15

Duration of Quiz :- 15 min

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1) Two liquids ‘A’ and ‘B’ have vapour pressure of 0.685 bar and 0.264 bar respectively. In an ideal solution of the two, the mole fraction of ‘A’ at which the two liquids have equal partial pressure is :

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2) PA and PB are the vapour pressure of pure liquid components A and B respectively of an ideal binary solution. If ‘XA‘ represents the mole fraction of component ‘A’, the total vapour pressure of the solution will be:

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3) Calculate the mass of urea (NH2CONH2) required in making 2.5 Kg of 0.25 molal aqueous solution.

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4) The freezing point of 1 % solution of lead nitrate in water will be :

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5) The mole fraction of solute in 2.5 molal aqueous solution is :

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6) An aqueous solution boils at 100.512 °C. The freezing point of the solution is (Kf = 1.86 K Kg mol−1 and Kb = 0.512 K Kg mol−1) :

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7) At 298 K, the total pressure of an ideal solution obtained by mixing 3 moles of ‘A’ and 2 moles of ‘B’ is 184 torr. What is the vapour pressure (in torr) of pure ‘B’ at the same temperature ? (Vapour pressure of ‘A’ at 298 K is 200 torr)

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8) The molarity of a solution containing 5.0 gm of NaOH in 250 mL solution is :

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9) A 6.9 M solution of KOH in water contains 30% by mass of KOH. The density of KOH solution is :

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10) Lowering of vapour pressure of an aqueous solution of a non-volatile, non-electrolyte 1 molal aqueous solution at 100 °C is:

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11) The volume of 10 N and 4 N HCl required to make 1 L of 7 N HCl are :

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12) Which of the following can be measured by the Ostwald-Walker dynamic method ?

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13) 138 g of ethyl alcohol is mixed with 72 g of water. The ratio of mole fraction of alcohol to water is.

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14) Two bottles ‘A’ and ‘B’ contains 1 M and 1 m aqueous solution of H2SO4 respectively.

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15) How many gram of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M nitric acid. The concentrated acid is 70% HNO3.

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