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Ionic Equilibrium 1 Mark Book Back Question Paper With Answer Key

12th Standard

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Chemistry

Time : 00:23:00 Hrs
Total Marks : 23

    Multiple Choice Question 

    23 x 1 = 23
  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. Following solutions were prepared by mixing different volumes of NAOH of HCL different concentrations
    1) 60 mL\(\frac{M}{10}\)HCl + 40mL\(\frac{M}{10}\)NaOH
    2) 55 mL\(\frac{M}{10}\)HCl + 45mL\(\frac{M}{10}\)NaOH
    3) 75 mL\(\frac{M}{5}\)HCl + 25mL\(\frac{M}{5}\)NaOH
    4) 100 mL\(\frac{M}{10}\)HCl + 100mL\(\frac{M}{10}\)NaOH
    pH of which one of them will be equal to 1?

    (a)

    (iv)

    (b)

    (i)

    (c)

    (ii)

    (d)

    (iii)

  3. The solubility of BaSO4 in water is 2.42 × 10-3gL-1 at 298K. The value of its solubility product(Ksp) will be (Given molar mass of BaSO4 =233g mol-1)

    (a)

    1.08 × 10-14mol2L-2

    (b)

    1.08 × 10-12mol2L-2

    (c)

    1.08 × 10-10mol2L-2

    (d)

    1.08 × 10-8mol2L-2

  4. 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

  5. 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

  6. 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

  7. Which of the following fluro compounds is most likely to behave as a Lewis base?

    (a)

    BF3

    (b)

    PF3

    (c)

    CF4

    (d)

    SiF4

  8. Which of these is not likely to act as Lewis base?

    (a)

    BF3

    (b)

    PF3

    (c)

    CO

    (d)

    F

  9. 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

  10. The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5NH) in a 0.10M aqueous pyridine solution _______.(Kb for C5H5N = 1.7×10-9) is 

    (a)

    0.006%

    (b)

    0.013%

    (c)

    0.77%

    (d)

    1.6%

  11. Equal volumes of three acid solutions of pH 1,2 and 3 are mixed in a vessel. What will be the H+ ion concentration in the mixture?

    (a)

    3.7 × 10-2

    (b)

    10-6

    (c)

    0.111

    (d)

    none of these

  12. The solubility of AgCl (s) with solubility product 1.6 × 10-10 in 0.1M NaCl solution would be _______.

    (a)

    1.26 × 10-5M

    (b)

    1.6 × 10-9M

    (c)

    1.6 × 10-11M

    (d)

    Zero

  13. If the solubility product of lead iodide is 3.2 × 10-8, its solubility will be _______.

    (a)

    2 × 10-3M

    (b)

    4 × 10-4M

    (c)

    1.6 × 10-5M

    (d)

    1.8 × 10-5M

  14. MY and NY3, are insoluble salts and have the same Ksp values of 6.2 × 10-13 at room temperature. Which statement would be true with regard to MY and NY3?

    (a)

    The salts MY and NY3 are more soluble in 0.5M KY than in pure water

    (b)

    The addition of the salt of KY to the suspension of MY and NY3 will have no effect on their solubility’s

    (c)

    The molar solubilities of MY and NY3 in water are identical

    (d)

    The molar solubility of MY in water is less than that of NY3

  15. What is the pH of the resulting solution when equal volumes of 0.1M NaOH and 0.01M HCl are mixed?

    (a)

    2.0

    (b)

    3

    (c)

    7.0

    (d)

    12.65

  16. The dissociation constant of a weak acid is 1 × 10-3. In order to prepare a buffer solution with a pH = 4, the [Acid]/[Salt] ratio should be _______.

    (a)

    4:3

    (b)

    3:4

    (c)

    10:1

    (d)

    1:10

  17. The pH of 10-5M KOH solution will be _______.

    (a)

    9

    (b)

    5

    (c)

    19

    (d)

    none of these

  18. H2PO4- the conjugate base of _______.

    (a)

    PO43−

    (b)

    P2O5

    (c)

    H3PO4

    (d)

    HPO42-

  19. Which of the following can act as Lowery – Bronsted acid well as base?

    (a)

    HCl

    (b)

    SO42−

    (c)

    HPO42−

    (d)

    Br-

  20. The pH of an aqueous solution is Zero. The solution is _______.

    (a)

    slightly acidic

    (b)

    strongly acidic

    (c)

    neutral

    (d)

    basic

  21. The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by _______.

    (a)

    \([{ H }^{ + }]=\frac { { K }_{ a }[acid] }{ [salt] } \)

    (b)

    \([{ H }^{ + }]={ K }_{ a }[salt]\)

    (c)

    \([{ H }^{ + }]={ K }_{ a }[acid]\)

    (d)

    \([{ H }^{ + }]=\frac { { K }_{ a }[salt] }{ [acid] } \)

  22. Which of the following relation is correct for degree of hydrolysis of ammonium acetate?

    (a)

    \(h=\sqrt { \frac { { K }_{ h } }{ C } } \)

    (b)

    \(h=\sqrt { \frac { { K }_{ a } }{ K_b } } \)

    (c)

    \(h=\sqrt { \frac { { K }_{ w } }{ { K }_{ a }.{ K }_{ b } } } \)

    (d)

    \(h=\sqrt { \frac { { { K }_{ a }.{ K }_{ b } } }{ { K }_{ w } } } \)

  23. Dissociation constant of NH4OH is 1.8 x 10-5  the hydrolysis constant of NH4Cl would be _______.

    (a)

    1.8 × 10-19

    (b)

    5.55 × 10-10

    (c)

    5.55 × 10-5

    (d)

    1.80 × 10-5

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