Chemistry QuestionsChemistry Xii – Solutions Questions for CBSE Class 12th

Chemistry Xii – Solutions Questions for CBSE Class 12th

Assuming each salt to be 90% dissociated which of the following will have the highest osmotic pressure?

The osmotic pressure of a solution containing 0.1 mol of solute per litre at 273 K is ——- atm.

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    Benzene freezes at 5.5ºC. The temperature at which a solution of 10 g of C 4 H 10 in 200 g of Benzene freeze is ºC. (The molal freezing point depression constant of Benzene is 5.12ºC/m)

    One mole of a solute A is dissolved in a given volume of a solvent. The association of the solute take place as follows n A ⇌ A n . If a is the degree of association of A, the Van’t Hoff factor i is expressed as

    A 5% solution of cane sugar (molecular weight = 342) is isotonic with a 1% solution of substance X. The molecular weight of X is

    How much amount of NaCl should be added to 600 g of water ρ = 1.00    g / m L to decrease the freezing point of water to – 0.2°C ? ( The freezing point depression constant for water =2 K kg mol − 1 )

    Which of the following statements is false?

    A decimolar solution of K 4 Fe CN 6 at 300K is 50% dissociated, then its osmotic pressure is

    Which of the following liquid pairs shows a positive deviation from Raoults law ?

    10.0 g of glucose ( π 1 ), 10.0 g of urea ( π 2 ), and 10.0 g of sucrose ( π 3 ) are dissolved in 250.0 mL of water at 273 K ( π = osmotic pressure of a solution). The relationship between the osmotic pressure of the solutions is

    What mass of urea be dissolved in 171 g of water so as to decrease the vapour pressure of water by 5%?

    The Van’t Hoff factor for a 0.1 M Al 2 (SO 4 ) 3 solution is 4.20. The degree of dissociation is

    An aqueous solution containing an ionic salt having molality equal to 0.19 freezes at -0.704 ° C. The Van’t Hoff factor of the ionic salt nearly is (K f for water = 1.86 K m -1 )

    The ratio of the value of any colligative property for KCI solution to that of sugar solution is

    Which of the following solutions has minimum freezing point?

    The osmotic pressure of a 5% (weight/volume) solution of cane sugar at 150 ° C is X (nearest single digit whole number)

    The osmotic pressure of a solution (density is 1 g mL -1 ) containing 3 g of glucose (molecular weight – 180) in 60 g of water at 15 ° C is

    The molal freezing point constant of water is 1.86 K m -1 . If 342 g of cane sugar (C 12 H 22 O 11 ) is dissolved in 1000 g of water, the solution will freeze at – X 0 C, the value of X is

    18 g of glucose (Mol.wt = 180) is added to (X) moles of water. The vapour pressure of water in torr for this aqueous solution is 752.4 torr. The value of (X) is ————————-(nearest whole number)

    HgI 2 is added to aqueous KI solution, then the vapour pressure of new solution is,

    At 35ºC, the vapour pressure of CS 2 , is 512 mm Hg and that of acetone is 344mm Hg. A solution of CS 2 in acetone has a total vapour pressure of 600mm Hg. The false statement amongst the following is:

    Two open beakers one containing a solvent and the other containing a mixture of that solvent with a non volatile solute are together sealed in a container. Over time:

    A cylinder containing an ideal gas (0.1 mol of 1.0 d m 3 ) is in thermal equilibrium with a large volume of 0.5 molal aqueous solution of ethylene glycol at its freezing point. If the stoppers S 1 a n d S 2 (as shown in the figure) are suddenly withdrawn, the volume of the gas in litres equilibrium is achieved will be ( Given, K f water = 2 .0   K   kg   mol − 1 R = 0 .08   dm 3 atm   K − 1 mol − 1 )

    Henry’s constant (in kbar) for four gases α , β , γ and δ in water at 298 K is given below : density of water = 10 3 kg m – 3 at 298 K This table implies that :

    The mole fraction of glucose C 6 H 12 O 6 in an aqueous binary solution is 0.1. The mass percentage of water in it, to the nearest integer, is .

    Insulin is dissolved in suitable solvent and the osmotic pressure in atm of solutions at various concentration is measured at 20°C. The slope of the plot of p against C is found to be 4.65 × 10 -3 . The molecular weight of insulin is 5.17 × 10 x . Then ‘x’ is

    Mixture of volatile components A and B has total vapour pressure (in Torr) p = 254 − 119    x A , where x A is mole fraction of A in mixture. Hence p A ∘ and p  B ∘ are (in Torr)

    Determine the amount (in mg) of CaCl 2 (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27°C. (Take RT = 25)

    The Henry’s law constant does not depend upon

    which of the following is a colligative properties

    Which will form maximum boiling azeotrope?

    An aqueous solution freezes at -2.55 ° C. What is its boiling point K b H 2 O = 0. 52 K m -1 ; K f (H2O) = 1.86 K m -1

    Which of the following represents correctly the changes in thermodynamic properties during the formation of I mole of an ideal binary solution?

    0.6 g of a solute is dissolved in 0.1 L of a solvent which develops an osmotic pressure of 1.23 atm at 27 ° C. The molecular weight of the solute is nearly

    The vapour pressure at a given temperature of an ideal solution containing 0.2 mol of non-volatile solute and 0.8 mol of a solvent is 60 mm of Hg. The vapour pressure of the pure solvent at the same temperature will be

    The degree of dissociation α of a weak electrolyte is

    Arrange the following as directed: (Q.79-82) Increasing order of boiling points. I. 0.001 m NaCl II. 0.001 m urea III. 0.001 m MgCl 2 IV. 0.001 m CH 3 COOH

    The relative lowering of vapour pressure is equal to the mole fraction of the non-volatile solute. This statement was given by

    The colligative properties of a solution depend on

    The freezing point of 1 m NaCl solution assuming NaCl to be 100% dissociated in water is – X 0 C . The value of X is ( K f =1.86 K .m -1 )

    The osmotic pressure of equimolar solutions of BaCl 2 , NaCl, and glucose follow the order

    The elevation in boiling point of 1 molal aqueous solution of urea is X K. The elevation in boing point of 0.2 molal aqueous solution of Aluminium sulphate is (Assuming complete ionization)

    VantHoff factor for 0.1 M MgSO 4 solution is 1.42 and for 0.001M MgSO 4 solution is 1.92. What is VantHoff factor for 0.01M MgSO 4 solution is

    The freezing point of a solution composed of 10.0 g of KCl in 100 g of water is -4.5 o c. Calculate the van’t Hoff factor i, for this solution.(K f =1.86Kkgmol -1 ) (up to 1 decimal)

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