2 & 3 Marks
1. What is a Solution?
2. What is a Solvent and Solute? Explain with an example.
3. What is Aqueous solution and Non-aqueous solution? Give examples.
4.
What
is a Gaseous Solution?
Give
examples.
5. What is a Liquid Solution? Give examples.
6. What is a Solid Solution? Give examples.
7.
Mention the Different concentration units.
8. What is meant by Concentration of a solution?
9. Define
Molality.
10.
Define Molarity.
11.
Define Normality.
12.
Define Formality.
13.
Define Mole fraction (of a component).
14.
Define Mass percentage.
15.
Define Volume percentage.
16.
Define Mass by volume percentage.
17.
Define Parts per million (ppm).
18. What is a Standard solution? Or What is a Stock solution?
19. How can
you prepare a Standard solution of required concentration?
20. What is a Working standard?
21. How can
you prepare a Working standard
of required concentration? Or
How can you prepare solutions of
required concentrations by diluting the Stock solution?
22. Give the expression for the calculation of Necessary
volumes of the Stock solution and Final volume and explain the
terms.
23.
What
are the Advantages of using Standard solutions?
24.
What
is the Solubility of a solute?
25.
What
is a Saturated solution?
26. Define Solubility.
27.
You
are provided with a solid ‘A’ and three solutions of A dissolved in water - one
Saturated, one Unsaturated, and
one Super saturated. How would you determine which solution is which?
28.
What
are the Factors influencing the Solubility (of a Solute in a Solvent)?
29. Explain the effect of Temperature of a Solid solute in Liquid
solvent on the Solubility.
30. Explain the effect of Temperature of a Gaseous solute in Liquid
solvent on the Solubility.
31. Show with an activity that there is a Decrease in Solubility
of gases in solution with Increase in Temperature. Or Show with an
activity that the Increase
in Temperature Decreases the Dissolution of gaseous molecules in Liquid Solvents.
32. Explain the effect of Pressure on the Solubility.
33. What are the Factors influencing the Solubility of a Gas in a Liquid?
34.
Define
Henry’s law. Or
State Henry’s law.
35.
Which
properties are related in Henry’s Law?
36.
What
are the Limitations of Henry’s law?
37.
Explain
why the aquatic species are more comfortable in cold water during winter season
rather than warm water during
the summer.
38.
What
is Evaporation?
39.
What
is Condensation?
40. What is a Vapour pressure of liquid?
41. What is a
Binary solution? Give examples.
42. State Raoult Law.
43. Which properties are related in Raoult Law?
44. What is Relative lowering of vapour pressure?
45. Compare Raoult’s law and Henry’s law.
46. What are Ideal solutions? Give examples.
47. Mention
the characteristics
of Ideal solutions.
48. What are Non-ideal / Real solutions? Give examples.
49.
When
will Non-ideal /
Real solutions show Positive deviation from Rauolt's Law? Give examples.
50.
When
will Non-ideal /
Real solutions show Negative deviation from Rauolt's Law? Give examples.
51. Mention
the
characteristics of Non-ideal /
Real solutions.
52.
What
are the factors responsible for deviation from Raoult’s law / ideal behavior?
53.
Solute-solvent
interactions are responsible for deviation from Raoult’s law / ideal behavior -
Explain.
54. Dissociation of solute is responsible for deviation from
Raoult’s law /
ideal behavior - Explain.
55. Association of solute is responsible for deviation from
Raoult’s law /
ideal behavior - Explain.
56. Temperature is responsible for deviation from Raoult’s
law / ideal
behavior - Explain.
57. Pressure is responsible for deviation from Raoult’s law / ideal behavior -
Explain.
58. Concentration is responsible for deviation from Raoult’s
law / ideal
behavior - Explain.
59. What are Colligative properties? What are they?
60. What is a Boiling point?
61. What is Elevation of boiling point?
62. Define Molal boiling point elevation constant. Or Define
Ebullioscopic constant.
63. What is a Freezing point?
64. What is Depression of freezing point?
65. Define Molal freezing point depression constant. Or Define Cryoscopic
constant.
66. What is Molal depression constant? Does it depend on
nature of the solute?
67. Which
solution has the lower freezing point? 10 g of Methanol (CH3OH)
in 100 g of water (or) 20 g of Ethanol (C2H5OH)
in 200 g of water.
68. What
is Osmotic pressure?
69. What are the
Significances of Osmotic pressure?
70. What
are Isotonic solutions? Or
Define
the term ‘Isotonic solution’.
71.
What is meant by van’t Hoff factor? Or Define Van't
Hoff factor.
72.
Calculate
Degree of dissociation / association related to Van't Hoff factor.
5 Marks
1. Classify solutions based on the Physical state of the
Solute and Solvent. Give examples.
2. Explain the effect of
Nature
of solute and solvent on the Solubility.
3. Explain Henry’s law.
4. Obtain expression for Total pressure formed when a
volatile liquid is dissolved in solvent.
5. Obtain expression for Lowering of vapour pressure when Non-volatile
solute is dissolved in solvent.
6. Explain the deviation of Real / Non-ideal solutions from Raoult’s Law.
7.
Explain
the factors responsible for deviation from Raoult’s law / ideal behavior.
8. How will you determine the molar mass of a Non-volatile
solute from relative lowering of vapour pressure?
9.
How
will you determine the Molar mass of a Non-volatile solute from Elevation of boiling point?
10. How will you determine the Molar mass of a Non-volatile
solute from Depression in
freezing point?
11. How will you determine the Molar mass of a Non-volatile
solute from Osmotic
pressure?
12.
Explain Reverse osmosis.
13. Write a note on
Abnormal molar mass. Or
Explain
the Abnormal colligative properties.
14. Write a note on Van't Hoff
factor.
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