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Ionic Equilibrium

12th Chemistry - Ionic Equilibrium Model Question Paper

Ionic Equilibrium Model Question Paper

12th Standard

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Chemistry

Time : 00:45:00 Hrs
Total Marks : 35
    5 x 1 = 5

  1. Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.24 ×10-4mol L-1 solubility product of Ag2C2O4 is_______.

    (a)

    2.42 × 10-8mol3L-3

    (b)

    2.66 × 10-12mol3L-3

    (c)

    4.5 × 10-11mol3L-3

    (d)

    5.619 × 10-12mol3L-3

  2. pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2 _______.

    (a)

    0.5 × 10-15

    (b)

    0.25 × 10-10

    (c)

    0.125 × 10-15

    (d)

    0.5 × 10-10

  3. Conjugate base for Bronsted acids H2O and HF are _______.

    (a)

    OH- and H2FH+, respectively

    (b)

    H3O+ and F-, respectively

    (c)

    OH- and F-, respectively

    (d)

    H3O+ and H2F+, respectively

  4. Which will make basic buffer?

    (a)

    50 mL of 0.1M NaOH+25mL of 0.1M CH3COOH

    (b)

    100 mL of 0.1M CH3COOH+100 mL of 0.1M NH4OH

    (c)

    100 mL of 0.1M HCl+200 mL of 0.1M NH4OH

    (d)

    100 mL of 0.1M HCl+100 mL of 0.1M NaOH

  5. The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively _______.

    (a)

    acidic, acidic, basic

    (b)

    basic, acidic, basic

    (c)

    basic, neutral, basic

    (d)

    none of these

    6. 3 x 2 = 6

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

  7. A lab assistant prepared a solution by adding a calculated quantity of HCl gas 250C 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. 3 x 3 = 9

  9. Define pH.

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

  11. 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.

    12. 3 x 5 = 15

  12. Ksp of AgCl is \(1.8\times10^{-10}\). Calculate molar solubility in 1 M AgNO3

  13. Write the expression for the solubility product of Hg2Cl2 .

  14. Will a precipitate be formed when 0.150 L of 0.1M Pb(NO3)2 and 0.100L of 0.2 M NaCl are mixed? \(K_{sp}\ (PbCl_{2})=1.2\times10^{-5}\).

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