EAMCET Chemistry Crash Course: 100 One-Liners on Solutions!

Here are 100 one-liner questions and answers based on NCERT’s Second Year Intermediate Chemistry Part 1, Unit 1: Solutions, tailored for EAMCET/EAPCET exam preparation:

EAMCET Chemistry: Basic Concepts & Types of Solutions

1. What is a solution?
   A homogeneous mixture of two or more substances.
2. Give an example of a solid-gas solution.
   Hydrogen adsorbed on palladium.
3. What is the solvent in an aqueous sugar solution?
   Water.
4. Define binary solution.
   A solution with two components (solute + solvent).
5. Give an example of a liquid-liquid solution.
   Ethanol in water.

EAMCET Chemistry: Concentration Terms

6. Define molarity (M).
   Moles of solute per liter of solution.
7. What is molality (m)?
   Moles of solute per kg of solvent.
8. Which concentration term is temperature-dependent?
   Molarity (volume changes with temperature).
9. Define mole fraction.
   Ratio of moles of a component to the total moles in the solution.
10. What is ppm (parts per million)?
    Mass of solute (in mg) per kg of solution.

EAMCET Chemistry: Solubility of Solids & Liquids

11. What factors affect the solubility of a solid in a liquid?
    Temperature and nature of solute/solvent.
12. How does temperature affect the solubility of most solids?
    Increases with temperature.
13. What is the effect of pressure on the solubility of solids in liquids?
    Negligible effect.
14. Define saturated solution.
    A solution in which no more solute can dissolve at a given temperature.
15. What is a supersaturated solution?
    A solution containing more solute than its saturation limit (unstable).

EAMCET Chemistry: Henry’s Law & Gas Solubility

16. State Henry’s law.
    The solubility of a gas in a liquid is directly proportional to the pressure of the gas.
17. Give the mathematical form of Henry’s law.
    P = Kₕ·X (P = pressure, Kₕ = Henry’s constant, X = mole fraction).
18. What is the effect of temperature on gas solubility?
    Decreases with increasing temperature.
19. Why do soda bottles fizz upon opening?
    Due to decreased pressure (Henry’s law).
20. Which gas obeys Henry’s law most accurately?
    Inert gases like N₂, O₂, etc.

EAMCET Chemistry: Raoult’s Law & Vapour Pressure

21. State Raoult’s law for a volatile solute.
    Partial vapour pressure of a component = mole fraction × pure vapour pressure.
22. What is an ideal solution?
    A solution that obeys Raoult’s law at all concentrations.
23. Give an example of an ideal solution.
    Benzene + Toluene.
24. What is a non-ideal solution?
    A solution that deviates from Raoult’s law.
25. What is positive deviation from Raoult’s law?
    Vapour pressure > expected, A-B interactions weaker than A-A/B-B (e.g., ethanol + water).
26. What is negative deviation from Raoult’s law?
    Vapour pressure < expected, A-B interactions stronger than A-A/B-B (e.g., chloroform + acetone).

EAMCET Chemistry: Colligative Properties

27. What are colligative properties?
    Properties depending on the number of solute particles, not their nature.
28. List four colligative properties.
    1. Lowering of vapour pressure, 2. Boiling point elevation, 3. Freezing point depression, 4. Osmotic pressure.
29. Define relative lowering of vapour pressure.
    (P° – P)/P° = X₂ (mole fraction of solute).
30. What is the formula for boiling point elevation?
    ΔT_b = K_b·m (K_b = ebullioscopic constant, m = molality).
31. Why does adding salt increase boiling point?
    Due to boiling point elevation (colligative property).
32. What is freezing point depression?
    ΔT_f = K_f·m (K_f = cryoscopic constant).
33. Why is salt sprinkled on icy roads?
    To lower the freezing point of water (freezing point depression).

EAMCET Chemistry: Osmosis & Osmotic Pressure

34. Define osmosis.
    Movement of solvent molecules through a semi-permeable membrane from low to high concentration.
35. What is osmotic pressure (π)?
    Pressure required to prevent osmosis.
36. Give the van’t Hoff equation for osmotic pressure.
    π = CRT (C = molarity, R = gas constant, T = temperature).
37. What are isotonic solutions?
    Solutions with the same osmotic pressure.
38. Define hypertonic and hypotonic solutions.
    Hypertonic: higher osmotic pressure; Hypotonic: lower osmotic pressure.
39. What is reverse osmosis?
    Applying pressure > osmotic pressure to force solvent from high to low concentration (used in water purification).
40. How is reverse osmosis used in desalination?
    To remove salts from seawater by applying high pressure.

EAMCET Chemistry: Abnormal Molar Mass & Van’t Hoff Factor

41. What is the van’t Hoff factor (i)?
    Ratio of observed colligative property to normal colligative property.
42. What is the value of ‘i’ for NaCl in water?
    ~2 (NaCl → Na⁺ + Cl⁻).
43. What is the ‘i’ value for glucose?
    1 (does not dissociate).
44. What causes abnormal molar mass?
    Dissociation/association of solute particles.
45. Give an example of solute association.
    Benzoic acid in benzene (forms dimers).

Applications & Miscellaneous

46. Why is ethylene glycol added to car radiators?
    To lower the freezing point of water (antifreeze).
47. What is edema?
    Swelling due to excess fluid in tissues (due to low osmotic pressure in blood).
48. Why are intravenous (IV) fluids isotonic with blood?
    To prevent cell damage (no osmosis occurs).
49. What is the effect of adding sugar on the boiling point of water?
    Boiling point increases (elevation).
50. What is the relationship between osmotic pressure and concentration?
    Directly proportional (π ∝ C).

EAMCET Chemistry: Numerical & Conceptual

51. If molality = 1 m, what is the mole fraction of solute in a dilute solution?
    ≈ 0.018 (for water as solvent).
52. Which has higher boiling point: 1M glucose or 1M NaCl?
    1M NaCl (i=2, more particles).
53. What happens to osmotic pressure if temperature increases?
    Increases (π ∝ T).
54. Which colligative property is used to determine molar mass of polymers?
    Osmotic pressure.
55. What is the unit of Henry’s constant (Kₕ)?
    bar or atm (depending on pressure unit).

Here are the remaining one-liner EAMCET/EAPCET-focused questions on Solutions (Unit 1, NCERT Chemistry Part 1):

Van’t Hoff Factor & Abnormal Molar Mass (Continued)

56. What is the ‘i’ value for AlCl₃ in water?
    ~4 (AlCl₃ → Al³⁺ + 3Cl⁻).
57. Why does acetic acid show ‘i’ < 1 in benzene?
    Due to dimer formation (association).
58. What is the relationship between ‘i’ and degree of dissociation (α)?
    i = 1 + (n−1)α (n = number of ions).
59. Calculate ‘i’ for 50% dissociation of KCl.
    i = 1 + (2−1)(0.5) = 1.5.
60. What is the ‘i’ value for a non-electrolyte like urea?
    1 (no dissociation).

EAMCET Chemistry: Solubility & Le Chatelier’s Principle

61. How does Le Chatelier’s principle apply to gas solubility?
    Increasing pressure increases solubility (Henry’s law).
62. Why does warm soda lose fizz faster than cold soda?
    Gas solubility decreases with temperature (Le Chatelier’s principle).
63. What happens to the solubility of CaCO₃ in water if CO₂ is added?
    Increases (forms soluble Ca(HCO₃)₂).
64. How does common ion effect reduce solubility?
    Adding a common ion shifts equilibrium to precipitate (e.g., AgCl in NaCl).

Applications in Daily Life

65. Why do fish die in warm water?
    Oxygen solubility decreases with temperature.
66. Why is CO₂ used in soft drinks?
    High solubility under pressure (Henry’s law).
67. What is the role of glycerol in moisturizers?
    Hygroscopic nature retains water (colligative property).
68. Why do alpine plants survive freezing temperatures?
    High solute concentration lowers freezing point.

EAMCET Chemistry: Numerical Problems (Conceptual)

69. If 0.1 M NaCl and 0.1 M glucose have the same boiling point, what is ‘i’ for NaCl?
    i = 1 (implies no dissociation, which is impossible; trick question).
70. Which has higher osmotic pressure: 0.1 M urea or 0.1 M NaCl?
    0.1 M NaCl (i=2 vs i=1 for urea).
71. If ΔT_b = 0.52°C for 1 m glucose, what is K_b for water?
    0.52 K·kg/mol.
72. What is the molar mass of solute if 5g in 100g water lowers FP by 0.5°C (K_f = 1.86)?
    M = (1000×K_f×w)/(ΔT_f×W) = (1000×1.86×5)/(0.5×100) = 186 g/mol.

EAMCET Chemistry: Distinguishing Ideal vs Non-Ideal Solutions

73. What is ΔH_mix for an ideal solution?
    Zero.
74. What is ΔV_mix for a non-ideal solution showing negative deviation?
    ΔV < 0 (volume decreases).
75. Which solution forms azeotropes?
    Non-ideal solutions (e.g., ethanol-water).

EAMCET Chemistry: Graph-Based Questions

76. What does a straight-line plot of P vs X for a solution indicate?
    Ideal behavior (obeys Raoult’s law).
77. In a P-X diagram, what does a curve above Raoult’s law line indicate?
    Positive deviation.
78. What does a minima in boiling point curve indicate?
    Maximum boiling azeotrope (negative deviation).

EAMCET-Specific Tricks

79. Which colligative property is best for measuring very low molar masses?
    Relative lowering of vapour pressure.
80. Why is molality preferred over molarity in colligative properties?
    Independent of temperature.
81. What is the order of osmotic pressure for equimolar solutions of NaCl, CaCl₂, urea?
    CaCl₂ (i=3) > NaCl (i=2) > urea (i=1).
82. Which gas’s solubility is most affected by temperature?
    CO₂ (high Kₕ value).

Medical & Biological Applications

83. Why does saline drip use 0.9% NaCl?
    Isotonic with blood plasma.
84. What happens to RBCs in hypotonic solution?
    Swell and burst (hemolysis).
85. What is lysis?
    Cell bursting due to osmosis.

EAMCET Chemistry: Advanced Concepts

86. What is the relationship between osmotic pressure and elevation in boiling point?
    Both depend on solute particle concentration.
87. Why does a non-volatile solute lower vapour pressure?
    Reduces solvent molecules at surface.
88. What is the effect of adding sugar on the freezing point of water?
    Freezing point decreases (depression).

Previous EAMCET Trends

89. Which law explains the “bends” in deep-sea divers?
    Henry’s law (N₂ solubility decreases during ascent).
90. What is the molality of 1 M NaCl solution (density ≈1 g/mL)?
    ≈1 m (for dilute solutions).
91. Which solution has the highest freezing point: 0.1 M glucose, 0.1 M NaCl, 0.1 M CaCl₂?
    0.1 M glucose (lowest ‘i’ value).

EAMCET Chemistry: Quick Recap (Definitions)

92. Define azeotrope.
    A mixture boiling at constant composition like a pure liquid.
93. What is ebullioscopic constant?
    Boiling point elevation per molal solution (K_b).
94. What is cryoscopic constant?
    Freezing point depression per molal solution (K_f).
95. Define semi-permeable membrane.
    Allows solvent but not solute to pass.

EAMCET Chemistry: Final Touches

96. Why is Hg used in pressure measurement in osmosis?
    High density allows visible pressure changes.
97. What is the role of sugar in jam preservation?
    High osmotic pressure prevents microbial growth.
98. What is the ‘i’ value for K₂SO₄ in water?
    ~3 (K₂SO₄ → 2K⁺ + SO₄²⁻).
99. Why do non-ideal solutions deviate from Raoult’s law?
    Due to differences in intermolecular forces (A-B ≠ A-A or B-B).
100. What is the key condition for reverse osmosis?
     Applied pressure > osmotic pressure (π).

These 100 one-liners cover all key concepts in the Solutions unit, with a focus on EAMCET/EAPCET exam patterns (numerical, conceptual, and application-based).

EAMCET Chemistry: Bonus Tip: For EAMCET, practice graph-based questions (Raoult’s law curves) and van’t Hoff factor calculations—they’re frequently asked!