Solubility Product Constant (Ksp) Definition and Calculation Quiz
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Questions and Answers

True or false: The solubility product constant (Ksp) is calculated by taking the product of the concentrations of the ions in a saturated solution of a sparingly soluble salt.

  • False
  • It depends on the stoichiometry of the salt
  • True (correct)
  • It depends on the solubility of the salt

    • What is the definition of the solubility product constant (Ksp)?

  • The rate at which a sparingly soluble salt dissolves in a given solvent
  • The product of the concentrations of the ions in a saturated solution of a sparingly soluble salt (correct)
  • The sum of the solubility constants of the ions in a solution
  • The ratio of the solute's concentration to the solvent's concentration

    • What is the solubility product constant (Ksp) expression for AgCl?

  • [Ag+] [Cl-] (correct)
  • [Ag+] [Cl-]^2
  • [Ag+]^2 [Cl-]
  • [Ag+]^2 [Cl-]^2

    • What is the solubility product constant (Ksp) expression for Ag2CrO4?

    <p>[Ag+]^2 [CrO4^2-]</p> Signup and view all the answers

    What is the general formula for the solubility product constant (Ksp) of a sparingly soluble salt AnBm?

    <p>Ksp_AnBm = [A^m+]^n [B^n-]^m</p> Signup and view all the answers

    Which statement is true regarding the effect of pH on solubility?

    <p>The solubility of many compounds decreases at low pH.</p> Signup and view all the answers

    True or false: Sparingly soluble salts will precipitate when the ionic product exceeds the solubility product constant (Ksp).

    <p>True</p> Signup and view all the answers

    In the presence of Ag+, which precipitate will form first when Cl- and I- ions are present?

    <p>AgI</p> Signup and view all the answers

    What is the correct relationship between the [Cl-] and [I-] ions for AgCl and AgI to precipitate simultaneously?

    <p>[Cl-] : [I-] = 1 : 106</p> Signup and view all the answers

    Which factor enhances the solubility of salts of weak acids?

    <p>Formation of free weak acid molecules</p> Signup and view all the answers

    If the solubility of Pb3(PO4)2 is 0.00014 g/L, what is the solubility product constant (Ksp) for Pb3(PO4)2?

    <p>$2.33 \times 10^{-16}$</p> Signup and view all the answers

    What is a characteristic of fractional precipitation when Ag+ is added to a solution containing both Cl- and I- ions?

    <p>Iodide will precipitate first due to lower solubility.</p> Signup and view all the answers

    If the solubility of AgCl is 1.05 x 10^-10 mol/L, what is the solubility product constant (Ksp) of AgCl?

    <p>1.05 x 10^-10</p> Signup and view all the answers

    If the solubility of Pb3(PO4)2 is 0.00014 g/L and its molar mass is 811.7 g/mol, what is the solubility product constant (Ksp) of Pb3(PO4)2?

    <p>1.5 x 10^-32</p> Signup and view all the answers

    What is the solubility of Mg(OH)2 in pure water if its Ksp is 3.4 x 10^-11 and molar mass is 58 g/mol?

    <p>0.00116 g/L</p> Signup and view all the answers

    According to Le Chatelier's principle, the presence of a common ion in a solution will:

    <p>Decrease solubility</p> Signup and view all the answers

    The theory of interionic attraction explains that a diverse ion in a solution:

    <p>Stabilizes the precipitate in its ionic form</p> Signup and view all the answers

    True or False: Increasing temperature increases the solubility of most inorganic salts.

    <p>True</p> Signup and view all the answers

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