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Ionic Equilibrium - Two Marks Study Materials

12th Standard EM

    Reg.No. :


Time : 00:45:00 Hrs
Total Marks : 30
    15 x 2 = 30
  1. What are lewis acids and bases? Give two example for each.

  2. Discuss the Lowery – Bronsted concept of acids and bases.

  3. Indentify the conjugate acid base pair for the following reaction in aqueous solution
    i) HS- (aq) + HF \(\rightleftharpoons \) F-(aq) + H2S(aq)
    ii) HPO2-+ SO32- \(\rightleftharpoons \) PO43-+HSO3-
    iii) NH4+ CO32-  \(\rightleftharpoons \) NH3+HCO3-

  4. Account for the acidic nature of HClO4. In terms of Bronsted – Lowry theory, identify its conjugate base.

  5. When aqueous ammonia is added to CuSO4 solution, the solution turns deep blue due to the formation of tetramminecopper (II) complex, \({ [Cu({ H }_{ 2 }O)] }_{ (aq) }^{ 2+ }\rightleftharpoons 4{ NH }_{ 3 }(aq)\rightleftharpoons { [Cu{ ({ NH }_{ 3 }) }_{ 4 }] }_{ (aq) }^{ 2+ }\) among H2O and NH3 Which is stronger Lewis base.

  6. The concentration of hydroxide ion in a water sample is found to be 2.5×10-6M. Identify the nature of the solution.

  7. A lab assistant prepared a solution by adding a calculated quantity of HCl gas 250C o to get a solution with [H3O+]= 4\(\times\)10-5M. Is the solution neutral (or) acidic (or) basic.

  8. Calculate the pH of 0.04 M HNO3 Solution.

  9. Define solubility product

  10. Calculate the concentration of OH- in a fruit juice which contains \(2\times10^{-3}\) M, H3O+ ion. Identify the nature of the solution.

  11. Calculate the pH of 0.001M HCl solution

  12. Calculate pH of 10-7M HCl

  13. The KW of a neutral solution is 10-12 at a particular temperature. What are its pH and pOH values?

  14. Calculate the ionisation constant for the conjugate base of HF. Ionisation constant of HF at 298 K is 6.8 X 10-4

  15. What are the limitations of Ostwald's dilution law?


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