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Chemical Equili...

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  • Question 1
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    An aqueous solution contains Ni2+ , Co2+ and Pb2+ ions at equal concentrations. The solubility product of NiS, PbS and CoS in water at 25oC are 1.4 × 10-24, 3.4 × 10-28 and 3 × 10-26, respectively. Indicate which of these ions will be precipitated first and last when sulphide concentration is progressively increased from zero?

  • Question 2
    4 / -1

    The solubility of AgC1 in 0.2 M NaCl is
    (Ksp of AgCl = 1.8 × 10-10)

  • Question 3
    4 / -1

    The solubility of AgCl is l × 10-5 mol/L. Its solubility in 0.1 molar sodium chloride solution is

  • Question 4
    4 / -1

    The solubility product of a sparingly soluble salt AX2 is 3.2 × 10-11. Its solubility (in mol/L) is

  • Question 5
    4 / -1

    When ammonium chloride is added to ammonia solution, the pH of the resulting solution will be

  • Question 6
    4 / -1

    Solubility of AgCl at 20°C is 1.435 × 10-3 g/ L. The solubility product of AgCl is

  • Question 7
    4 / -1

    At 30oC, the solubility of Ag2 CO3 (Ksp = 8 × 10-12) would be greatest in 1 L of

  • Question 8
    4 / -1

    The Ksp of Ca3 (PO4)2 is

  • Question 9
    4 / -1

    If solubility of calcium hydroxide is √3, then its solubility product will be

  • Question 10
    4 / -1

    The molar solubility (in mol L-1) of a sparingly soluble salt MX4 is 's'. The corresponding solubility product is KSP. S is given in terms of KSP by the relation

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