?Partial vapour pressure of a solution component is directly proportional to its mole fraction?. This statement is known as

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Question:
?Partial vapour pressure of a solution component is directly proportional to its mole fraction?. This statement is known as

1.Henrys law

2.Raoults law

3.Distribution law

4.Ostwalds dilution law.

Posted Date:-2021-09-30 18:15:10

More MCQS Questions and answers

  1. 0.1 M solution of glucose and 0.1 M solute of urea are placed on two sides of semipermeable membrane to equal heights. Which of the following is correct?
  2. 18% (W/V) solution of urea (Mol. Mass = 60) is
  3. 3% solution of glucose is isotonic with 1% solution of a non-volatile non-electrolyte substance. The molecular mass of the substance would be
  4. 34.2 gm of sugar (mol. wt. 342) is dissolved in 90 gm of water at the boiling point of water vapour pressure of solution at that very temperature will be
  5. 4 L of 0.2 M aqueous solution of KOH is mixed with 2 L of 0.5 M aqueous solution of KOH. The molarity of the resulting solution is
  6. 45% solution of glucose would be isotonic with respect to ?? solution of urea 9%
  7. 5.85 g of NaCl is dissolved in 500 ml of water. The molarity is
  8. ?Partial vapour pressure of a solution component is directly proportional to its mole fraction?. This statement is known as
  9. A 500 g tooth paste sample has 02 g fluoride concentration What is the concentration of fluoride in terms of ppm
  10. A colligative property depends upon
  11. A colligative property is
  12. A crystal of blue vitriol is placed in its saturated solution. Which of the following observations would you expect to make provided the temperature is constant? A super ? saturated solution will be formed
  13. A liquid is in equilibrium with its vapour at its boiling point. On the average the molecules of the two phases will have
  14. A non-volatile electrolyte dissolved in an aqueous solution in same molal proportion as non-electrolyte produces
  15. A non-volatile electrolyte dissolved in equimolal proportion as non-volatile non-electrolyte produces
  16. A solution containing one gram of substance in 100 ml of water is found to be isotonic with a solution of 3 grams of glucose in 100 ml of water. The molecular mass of the substance is
  17. A supersaturated solution is a metastable solution whose solute concentration
  18. According to Raoults law the relative lowering of vapour pressure of a solution of non-volatile solute is equal to mole fraction of solvent
  19. According to Raoults law for solution containing non-volatile solution the relative lowering of vapour pressure for solution is
  20. Acetic acid exists as dimers in benzene if on dissolving 1.65 gm of acetic acid in 100 gm of benzene the Vant Hoff factor i comes out to be 0.508 then extent of association of acetic acid in benzene is
  21. An aqueous solution containing 6 g of urea in 500 ml of solution has a density equal to 1.052. If the molecular mass of urea is 60 then the molality of solution is
  22. An aqueous solution of glucose is 10% in strength. The volume in which 1 gm mole of it is dissolved will be
  23. An azeotropic solution of two liquids has boiling point lower than ether when it
  24. At 298 K the vapour pressure of pure X is 50 mm Hg and that of pure Y is 60 mm Hg. If 1 mole of X and 1 mole of Y are mixed than vapour pressure of the solution was found out to be 57.5 mm Hg. The solution
  25. Certain substance trimerises when dissolved in a solvent A. The vant Hoffs factor i for the solutions is
  26. During molecular weight determination of non-volatile solute by cryoscopic method Beckmann Thermometer is used to determine the
  27. Ebullioscopic constant depends upon
  28. For a solution containing non-volatile solute the relative lowering of vapour pressure is 02 If the solution contains 5 moles in all which of the following are true?I Mole fraction of solute in the solution is02II No of moles of solute in the solution is 02III No of moles of solvent in the solution is 4IV Mole fraction of solvent is02
  29. For dilute solutions Raoults law states that
  30. For which of the following solutes i is greater than 1?
  31. Freezing point of an aqueous solution is 272.48 K. The osmotic pressure of the same solution at 310 K will be
  32. How many grams of a dibasic acid (Molecular mass = 200) should be present in 100 ml of its aqueous solution to give decinormal strength?
  33. Hydrochloric acid solutions A and B have concentrations 0.5 N and 0.1 N respectively. The volumes of solutions A and B required to make 2 litres of 0.2 N hydrochloric acid are
  34. If 0.1 M solution of glucose and 0.1 M solution of urea are placed on two sides of the semipermeable membrane to equal heights then it will be correct to say that
  35. In dilute solution the depression in freezing point is directly proportional to
  36. In the phenomenon of osmosis the semipermeable membrane allows the passage if
  37. In which of the following cases 1% aq Solution will have the lowest freezing point?
  38. Increasing the temperature of an aqueous solution will cause decrease in
  39. Isotonic solutions are those which have same
  40. Molality of a solution is the number of moles of solute in
  41. On dissolving 8.8 gm of non-volatile solute to 100 gm of water the vapour pressure of ice becomes 4.559 mm Hg. If vapour pressure of pure ice is 4.58 mm Hg than molecular weight of the substance should be
  42. or solutions the relation PV = nRT is called
  43. Osmotic pressure of a solution increases by
  44. Osmotic pressure of a solution of electrolyte does not depend onI. Nature of solute II. Nature of solventIII. Temperature IV. Molar conc. of solute.
  45. Osmotic pressure of blood is 7.65 atm at 310 K. An aqueous solution of glucose that will be isotonic with blood will be
  46. Raoults law for solutions containing non-volatile solute is concerned with lowering of
  47. Solutions with same vapour pressures are called
  48. The addition of a non-volatile solute to the solvent results in lowering of
  49. The amount of a solute required to prepare 10 litres of its decinomrla solution is
  50. The amount of gas dissolving in a given volume of the liquid decreases when
  51. The boiling point of a 0.1 molal aqueous solution of urea is 100.180C under one atmospheric pressure. The molal elevation constant of water is
  52. The cryoscopic constant for water is
  53. The enthalpy change on mixing water and ethanol at room temperature is
  54. The molality of 2% (w/w) aqueous solution of sodium chloride is
  55. The molality of an aqueous solution of NaOH containing 8 gram in 2 litres of solution is:
  56. The molarity of 6% (W/V) solution of acetic acid is
  57. The molarity of decinormal aqueous solution of sodium hydroxide is
  58. The molarity of pure water is
  59. The molarity of solution obtained by dissolving 001 moles of NaCl in 500 ml of solution is
  60. The molecular mass of ethyl alcohol is 46. The molality of a solution of ethyl alcohol in water containing 23.0 g of ethyl alcohol in 500 ml solution is
  61. The normality of a 2.3 M sulphuric acid solution is
  62. The number of moles of sodium hydroxide present in 25 L of 05 M aqueous solution is
  63. The osmotic pressure of a solution of benzoic acid in benzene is found to be half the expected value. This is due to the
  64. The ratio of elevation in boiling point of aqueous solution of sodium chloride to that of an aqueous solution of glucose of same molalities is approximately
  65. The solution that can distil with change in composition is called
  66. The vapour pressure of pure benzene at 298 K is 97.0 mm Hg. The vapour pressure of solution containing 10.0 gm of napthalene (mol. wt. 128) in 100 gm of benzene at 398 K will be
  67. The vapour pressure of water at room temperature is 23.8 mm Hg. The vapour pressure of an aqueous solution of mole fraction 0.1 is equal to
  68. The vapour pressure of water at room temperature is 30 mm. If the mole fraction of the solvent in solution is 0.9 the vapour pressure of aqueous solution at room temperature will be
  69. The volume of water that must be added to a mixture of 250 ml of M HCl and 750 ml of 2 M HCl to obtain 2.5 M solution is
  70. Two beakers contain 1 L and 250 ml of pure water respectively. What is same in them?
  71. Two liquids A and B form an ideal solution At 300 K the vapour pressure of a solution of 1 mole of A and x moles of B is 550 mm If the vapour pressures of pure A and B are 400 mm and 600 mm respectively then x is
  72. Two solutions A and B are separated by a semipermeable membrane. Solution B has greater vapour pressure than solution A. Water will flow from
  73. What volume of 0.8 M solution contains 0.1 mole of the solute?
  74. When 18 g of a compound was dissolved in 100 g of water the vapour pressure of the latter was lowered from 17.54 mm to 17.23 mm of mercury. The molecular mass of compound is
  75. When a saturated solution of sodium chloride is heated it becomes
  76. Which is an example of colligative property?
  77. Which of the following are not colligative properties?
  78. Which of the following change with increase in temperatureI Molality II MolarityIII Mole fraction IV Normality
  79. Which of the following is not a colligative property?
  80. Which of the following solutions will have highest value of depression in freezing point?
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