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Chemistry – Class XI

  2. Using half reaction method and oxidation number method balance the following equations:
  • Cl + MnO4–       ………        Cl2 + Mn2+     (acid medium)
  • NO2 + MnO4     ……..                 NO3 + Mn2+     (acid medium)
  • Mn2+ + ClO3–      …………          Mn4+    + Cl    (acid medium)
  • CrO3 + H2O2       ………           CrO42-+ H2O  (basic medium)
  • Fe2+ + H2O           ……..                     Fe3+    +  H2O  (basic medium)

MnO4–  + S2O32-     ……..                    MnO2 + SO42-  (basic medium


  1. What do you mean by dynamic nature of equilibrium?
  2. Define normal freezing point of a substance.
  3. What do you mean by ionic equilibrium?
  4. Define normal boiling point of a liquid.
  5. State Henry’s law.
  6. State the law of chemical equilibrium.
  7. How is equilibrium constant for the forward reaction related to equilibrium constant for the reverse reaction?
  8. Differentiate between homogeneous and heterogeneous equilibria.
  9. Derive the relationship between Kcand Kp
  10. If for a reaction Qc > Kc predict the direction of the reaction.
  11. Write the relationship between Kc and standard Gibb’s energy.
  12. State Le-Chatlier’s principle.
  13. What are the optimum conditions for the synthesis of ammonia?
  14. What are conjugate acid-base pairs?
  15. What are Lewis acids and Lewis bases?
  16. Define pH.
  17. How are Ka and Kb conjugate acid-base pair related?
  18. What are polyprotic acids?
  19. Why isKa2 of H2SO4 less than its Ka1?
  20. Arrange the following in the increasing order of acid strength                                 HF,HCl, HBr, HI                                                                                                                              . CH4, NH3, H2O, HF
  21. What is common ion effect?
  22. Name the two types of buffer solutions.
  23. Derive Henderson –Hasselbalch equation for an acid buffer.
  24. Define solubility product.
  25. Derive the relationship between solubility and solubility product of Zr3(PO4)4