1. Physical chemistry
    2. 1. The solid state
    2. Language of Chemistry
    3. Gaseous and Liquid states
    4. Stoichiometry
    5. Solutions
    6. Structure of Atom
    7. Chemical equilibrium
    8. Nuclear chemistry (Radioactivity)
    9. Ionic equilibrium
    10. Chemical Bonding
    11. Chemical kinetics
    12. Concepts of Acids, Bases and Salts
    13. Surface catalysis and Colloids
    14. Redox reactions
    15. Chemical energetics
    16. Volumetric analysis
    17. Electrochemistry
  2. Inorganic chemistry
    3. 18. Introduction
    19. Periodic table
    20. Hydrogen and its compounds
    21. General aspects of Metallergy
    22. Alkali metals
    23. Alkaline metals
    24. Boron family
    25. Carbon family
    26. Nitrogen family
    27. Oxygen family
    28. Fluorine family
    29. Inert gases
    30. Transition metals
    31. Coordination compounds
    32. Analytical chemistry
  3. Organic chemistry
    4. 33. Purification and analysis of organic compounds
    34. Nomenclature of Organic compounds
    35. Reaction Mechanisms
    36. Hydrocarbons
    37. Haloalkanes (Alkyl halides)
    38. Alcohol, Phenol and Ether
    39. Aldehyde and Ketones
    40. Carboxylic acids
    41. Compounds conatining Nitrogen
    42. Polymers
    43. Chemistry in daily life
Physical chemistry
9. Ionic equilibrium
1. pH of 10-12 M HCl is

[MOE Model]

  • 12.0
  • 2.0
  • 7.0
  • -12
2. The pH value of a solution of NaOH is 10. Assuming complete dissociation, the concentration of OH- ion is

[MOE 2062]

  • 10-10
  • 10-1
  • 10-4
  • None of above
3. Why is precipitate of AgCl obtained when a drop of AgNO3 is added to aqueous NaCl solution?

[MOE 2062]

  • Ionic product of AgCl > solubility product
  • Solubility product > ionic product of AgCl
  • Solubility product = ionic product of AgCl
  • Solubility product ≠ ionic product of AgCl
4. Ionic product of water is

[MOE 2060]

  • 101 moles/litre
  • 10-14 moles2/litre2
  • 10-7 moles/litre
  • 10-14 moles/litre
5. pH of 0.02 M NaOH is

[MOE 2063]

  • 1.7
  • 12.3
  • 10.3
  • 13.3
6. pH of 50 cc of 0.01 N HCl is decreased by
  • Adding 50 cc of 0.01 N HCl
  • Adding 50 cc of water
  • Adding 10 cc of 0.0001 N HCl
  • Adding 50 cc of 0.1 N HCl
7. 4 ml of 0.5 N HCl is mixed with 1 ml of 2 N KOH. The pH of resulting solution is

[MOE 2056]

  • 0
  • 7
  • 3
  • 10
8. Solubility of AB2 is x. Then the solubility product will be

[IOM 2007]

  • 4x3
  • 27x4
  • 108x5
  • 125x5
9. The solubility product of a sparingly soluble salt AB2 is 1.08 × 10-23 at 25°C. Its molar solubility is

[IOM 1996]

  • 3 × 10-8 M
  • 3 × 10-6 M
  • 3 × 10-4 M
  • 3 × 10-2 M
10. pH of a solution containing 2 g of sodium hydroxide per litre of water will be

[IOM 2005]

  • 2
  • 10
  • 10.7
  • 12.7
11. The highest pH value is shown by 0.1 M

[IOM 2008, MOE 2065]

  • H2SO4
  • NaOH
  • Ca(OH)2
  • Na2CO3
12. pH of 0.1% solution of NaOH is
  • 1
  • 10
  • 8.6
  • 12.4