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Set 4 of 10 · Questions 91-120 of 274

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JEE Main Chemistry · Ionic Equilibrium · Set 4 (Q91-120)

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  1. 91.
    The solubility product of at is . The value if, its aqueous and saturated solution is
    1. (1)5
    2. (2)7.5
    3. (3)9
    4. (4)13
  2. 92.
    At , the equilibrium constant. for the reaction is . The (in bar) at the same temperature is
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  3. 93.
    Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of the them will be equal to 1?
    1. (1)100 mL HCl + 100 mL NaOH
    2. (2)75 mL HCl + 25 mL NaOH
    3. (3)60 mL HCl + 40 mL NaOH
    4. (4)55 mL HCl + 45 mL NaOH
  4. 94.
    On increasing temperature, the equilibrium constant of exothermic and endothermic reactions, respectively
    1. (1)increases and decreases
    2. (2)decreases and increases
    3. (3)increases and increases
    4. (4)decreases and decreases
  5. 95.
    Equal volumes of acetic acid and sodium acetate are mixed. What is the of resultant solution? of acetic acid
    1. (1)4.85
    2. (2)4.65
    3. (3)4.75
    4. (4)7.0
  6. 96.
    An organic monobasic acid has dissociation constant . What is percent dissociation in it's solution?
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  7. 97.
    Solid Ba is gradually dissolved in 1.0 × M solution. At what concentration of will a precipitate begin to form ? ( for = 5.1 × )
    1. (1)5.1 × M
    2. (2)8.1 × M
    3. (3)8.1 × M
    4. (4)4.1 × M
  8. 98.
    for the conversion of oxygen to ozone at is , its standard Gibbs energy change in is approximately
    1. (1)229.8
    2. (2)114.9
    3. (3)-229.8
    4. (4)-114.9
  9. 99.
    of an aqueous solution of is
    1. (1)7
    2. (2)
    3. (3)
    4. (4)1
  10. 100.
    of a mixture of and is neutralised by of .
    What is the amount of present in the mixture?
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  11. 101.
    Which one of the following statements is not true?
    1. (1)Among halide ions, iodide is the most powerful reducing agent.
    2. (2)Fluorine is the only halogen that does not show a variable oxidation state.
    3. (3)HOCI is a stronger acid than HOBr.
    4. (4)HF is a stronger acid than .
  12. 102.
    For the reaction, the equilibrium pressure is . If conversion is , the value of , in atm is
    1. (1)4
    2. (2)1
    3. (3)0.5
    4. (4)2
  13. 103.
    Strongest conjugate base among the following is
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  14. 104.
    The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid
    is [Given of ]
    1. (1)2.57
    2. (2)5.57
    3. (3)3.57
    4. (4)4.57
  15. 105.
    At , the solubility product of is . What is its molar solubility in solution at same temperature?
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  16. 106.
    The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, of the acid is :
    1. (1)3 ×
    2. (2)1 ×
    3. (3)1 ×
    4. (4)1 ×
  17. 107.
    The buffer system which helps to maintain the of blood between 7.26 to 7.42 , is
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  18. 108.
    Identify for following equation according to Bronsted-Lowry theory
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  19. 109.
    In which of the following, the solubility of will be minimum?
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  20. 110.
    Conjugate acid and conjugate base of are respectively
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  21. 111.
    At the molar solubility of in solution is . The values of and are respectively (at of
    1. (1)
    2. (2)25,13
    3. (3)25,14
    4. (4)
  22. 112.
    At , the ionisation constant for anilinium hydroxide is . The hydrolysis constant of anilinium chloride is
    1. (1)
    2. (2)
    3. (3)
    4. (4)
  23. 113.
    pH of water is 7 at . If water is heated to ., it's pH will:
    1. (1)
    2. (2)concentration increases, concentration decreases
    3. (3)
    4. (4)
  24. 114.
    A buffer solution is prepared by mixing sodium acetate and acetic acid. If for acetic acid is 4.7. Find the .
    1. (1)3.0
    2. (2)4.0
    3. (3)5.0
    4. (4)2.0
  25. 115.
    of pure HCl was used to make an aqueous solution. 25.0 mL of solution is used when the HCl solution was titrated against it. The numerical value of is . (Nearest integer) Given: Molar mass of HCl and are 36.5 and respectively.
  26. 116.
    The pH of ammonium phosphate solution, if of phosphoric acid and of ammonium hydroxide are 5.23and 4.75 respectively, is
  27. 117.
    One liter buffer solution was prepared by adding 0.10 mol each of and in deionised water. The change in pH on addition of 0.05 mol of HCl to the above solution is . (Nearest integer)
    Given: of and
  28. 118.
    of molar mass is required to be dissolved in 1.0 L of water to produce a pH of 10.0 at 298 K. The value of is mg. (Nearest integer)
    (Given: is assumed to dissociate completely in )
  29. 119.
    The percentage dissociation of a salt solution at given temperature (van't Hoff factor ) is % (Nearest integer)
  30. 120.
    In order to prepare a buffer solution of sodium acetate is added to acetic acid. If theconcentration of acetic acid in the buffer is , the concentration of sodium acetate in thebuffer is .(Round off to the Nearest Integer).
    [Given: (acetic acid)