Test: Solutions (Chapter 9)

Multiple Choice Questions

  1. 1. A sample of matter with uniform properties and a fixed composition is called a:

  2. 2. In a solution, the substance present in the larger quantity is called the:

  3. 3. A solution containing a relatively small amount of solute is called:

  4. 4. Which concentration unit represents the weight of solute per 100 parts by weight of solution?

  5. 5. A 10% w/v glucose solution contains:

  6. 6. Molarity (M) is defined as the number of moles of solute dissolved per:

  7. 7. To prepare 1 Molar solution of glucose (C₆H₁₂O₆, Molar mass = 180 g/mol), you dissolve 180g of glucose in:

  8. 8. Molality (m) is defined as the number of moles of solute dissolved per:

  9. 9. Which concentration unit is independent of temperature?

  10. 10. Mole fraction (x) of a component is the ratio of its moles to:

  11. 11. The sum of mole fractions of all components in a solution is always equal to:

  12. 12. In a mixture of gases, the mole fraction of a gas is equal to its partial pressure divided by:

  13. 13. Parts per million (ppm) is typically used for:

  14. 14. To convert between different concentration units (like Molarity and %w/w), what additional information is often required?

  15. 15. Air is an example of which type of solution?

  16. 16. Sugar dissolved in water is an example of which type of solution?

  17. 17. Metal alloys like steel (carbon in iron) are examples of which type of solution?

  18. 18. The general solubility principle 'like dissolves like' refers to similarities in:

  19. 19. Why do ionic solids like NaCl typically dissolve well in polar solvents like water?

  20. 20. Liquids that mix in all proportions, like alcohol and water, are called:

  21. 21. When ether and water are mixed, they form two layers, each layer being a saturated solution of the other liquid. These layers are called:

  22. 22. The temperature at which two conjugate solutions merge into a single homogeneous phase is called the:

  23. 23. The critical solution temperature (upper consulate temperature) for the phenol-water system is approximately:

  24. 24. Water and benzene are examples of liquids that are practically:

  25. 25. An ideal solution is one that:

  26. 26. Which pair of liquids is most likely to form an ideal solution?

  27. 27. Raoult's law states that the vapour pressure of a solvent above a solution (p) is equal to:

  28. 28. The relative lowering of vapour pressure (Δp/p°) is equal to:

  29. 29. Relative lowering of vapour pressure depends on:

  30. 30. For a solution of two volatile liquids A and B, the total vapour pressure (Pt) is given by:

  31. 31. In fractional distillation of an ideal binary mixture, the vapour phase is always richer in the:

  32. 32. Liquid mixtures that distill with a change in composition are called:

  33. 33. Non-ideal solutions show deviations from Raoult's Law due to differences in:

  34. 34. A mixture that boils at a constant temperature without changing composition is called:

  35. 35. Solutions showing positive deviation from Raoult's law have vapour pressures:

  36. 36. A minimum boiling azeotrope is formed by solutions that show:

  37. 37. The ethanol-water system forms an azeotrope that boils at a temperature:

  38. 38. Solutions showing negative deviation from Raoult's law have vapour pressures:

  39. 39. A maximum boiling azeotrope is formed by solutions that show:

  40. 40. The HCl-water system forms an azeotrope that boils at a temperature:

  41. 41. A saturated solution is one where the dissolved solute is in equilibrium with:

  42. 42. Solubility is typically defined as the concentration of solute in a ___ solution at a specific temperature.

  43. 43. A graphical representation between temperature and solubility is called a:

  44. 44. Which type of solubility curve shows sharp breaks, indicating a change in the solid phase?

  45. 45. The solubility curve for Na₂SO₄·10H₂O changing to Na₂SO₄ is an example of a:

  46. 46. Which substance shows exceptional behaviour with its solubility decreasing as temperature increases?

  47. 47. Fractional crystallization is a technique used for:

  48. 48. Colligative properties depend primarily on the:

  49. 49. Which of the following is NOT considered a colligative property?

  50. 50. Why do 0.1 molal solutions of urea, glucose, and sucrose in water exhibit the same lowering of vapour pressure?

  51. 51. The molal boiling point elevation constant (Kb) depends on the:

  52. 52. The molal freezing point depression constant (Kf) is also known as the:

  53. 53. For colligative properties to be accurately observed, the solution should ideally be:

  54. 54. The presence of a non-volatile solute lowers the vapour pressure of a solvent because:

  55. 55. The formula M₂ = (p°/Δp) * (W₂M₁/W₁) is used to determine:

  56. 56. Elevation of boiling point (ΔTb) is directly proportional to:

  57. 57. The formula ΔTb = Kb * m relates boiling point elevation to:

  58. 58. The Landsberger's method is used to measure:

  59. 59. In the Landsberger method, the solvent in the inner tube is heated by:

  60. 60. The freezing point of a substance is the temperature where:

  61. 61. Adding a non-volatile solute to a solvent ___ the freezing point.

  62. 62. Depression of freezing point (ΔTf) is related to molality (m) by the equation:

  63. 63. The Beckmann's apparatus is used to measure:

  64. 64. The air jacket in the Beckmann's apparatus helps to ensure:

  65. 65. Ethylene glycol is used as antifreeze in car radiators because it:

  66. 66. Adding NaCl or KNO₃ to ice lowers its melting point, creating a:

  67. 67. The separation of solvent molecules to accommodate solute particles is generally an ___ process.

  68. 68. The interaction (mixing) between solute and solvent particles is generally an ___ process.

  69. 69. The overall enthalpy change when one mole of a substance dissolves in a specified amount of solvent is called the:

  70. 70. If ΔHsoln is positive, the dissolution process is:

  71. 71. If ΔHsoln is negative, the dissolution process is:

  72. 72. The energy required to separate one mole of a crystalline ionic compound into isolated gaseous ions is called:

  73. 73. The energy released when ions are surrounded by solvent molecules (like water) is called:

  74. 74. Which ion would likely have a higher (more negative) hydration energy?

  75. 75. The process where water molecules surround solute ions or molecules is called:

  76. 76. Crystalline substances containing chemically combined water in definite proportions are called:

  77. 77. In CuSO₄·5H₂O, how many water molecules are typically associated with the Cu²⁺ ion?

  78. 78. The reaction of ions from a salt with water, potentially changing the pH, is called:

  79. 79. Dissolving ammonium chloride (NH₄Cl) in water produces an acidic solution because:

  80. 80. Dissolving sodium acetate (CH₃COONa) in water produces a basic solution because:

  81. 81. Which type of salt generally does NOT undergo hydrolysis and forms a neutral solution?

  82. 82. Dissolving NaCl in water results in a solution that is:

Short Answer Questions

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