Ionic Equilibrium Three Marks Questions

12th Standard EM

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Chemistry

Time : 00:45:00 Hrs
Total Marks : 36
    12 x 3 = 36
  1. Define ionic product of water. Give its value at room temperature.

  2. Explain common ion effect with an example

  3. Derive an expression for Ostwald’s dilution law

  4. Define pH.

  5. Calculate the pH of 1.5\(\times\)10-3Msolution of Ba(OH)2

  6. 50ml of 0.05M HNO3 is added to 50ml of 0.025M KOH. Calculate the pH of the resultant solution.

  7. The Ka value for HCN is 10-9 . What is the pH of 0.4M HCN solution?

  8. Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that \(K_{a}=K_{b}=1.8\times10^{-5}\)

  9. Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base

  10. A solution of 0.10M of a weak electrolyte is found to be dissociated to the extent of 1.20% at 25oC . Find the dissociation constant of the acid.

  11. Calculate the pH of 0.1M CH3COOH solution. Dissociation constant of acetic acid is \(1.8\times10^{-5}\).

  12.  Fine the pH of a buffer solution containing 0.20 mole per litre sodium acetate and 0.18 mole per litre acetic acid. Ka for acetic acid is \(1.8\times10^{-5}\).

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