Solubility Equilibria and Ksp
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Questions and Answers

What is the effect of adding a soluble salt that contains one of the ions of the slightly soluble salt on the solubility of the slightly soluble salt?

  • It increases the solubility of the slightly soluble salt
  • It has no effect on the solubility of the slightly soluble salt
  • It decreases the solubility of the slightly soluble salt (correct)
  • It changes the solubility product of the slightly soluble salt

    • What happens to the equilibrium when Pb2+ is added to the solubility equilibrium of solid PbCrO4?

  • The equilibrium becomes undefined
  • The equilibrium shifts to the right
  • The equilibrium shifts to the left (correct)
  • The equilibrium remains unchanged

    • What is the unit of molar solubility?

  • Grams per liter (g/L)
  • Grams per kilogram (g/kg)
  • Moles per kilogram (mol/kg)
  • Moles per liter (M) (correct)

    • What is the solubility product for calcium oxalate?

    <p>2.3 x 10^-9</p> Signup and view all the answers

    What is the effect of the common-ion effect on the solubility product of the slightly soluble salt?

    <p>It has no effect on the solubility product</p> Signup and view all the answers

    Why does the addition of Pb(NO3)2 to the solubility equilibrium of solid PbCrO4 decrease the solubility of PbCrO4?

    <p>Because the addition of Pb2+ ions shifts the equilibrium to the left</p> Signup and view all the answers

    What is the purpose of calculating the molar solubility of a slightly soluble salt?

    <p>To determine the amount of salt that can dissolve in a given volume of solution</p> Signup and view all the answers

    What is the condition necessary for the common-ion effect to occur?

    <p>A soluble salt that contains one of the ions of the slightly soluble salt must be added</p> Signup and view all the answers

    What is molar solubility in the context of a saturated solution?

    <p>The maximum amount of solute dissolved per liter of solution</p> Signup and view all the answers

    Under what condition can the Ksp values of different compounds be meaningfully compared?

    <p>When the compounds have the same dissociation stoichiometry</p> Signup and view all the answers

    What does the Ksp represent for a compound like calcium oxalate in a saturated solution?

    <p>The equilibrium constant for the dissolution reaction</p> Signup and view all the answers

    If a saturated solution of calcium oxalate produces a residue of 0.0061 g after evaporation, what information can be calculated?

    <p>The molar solubility of calcium oxalate</p> Signup and view all the answers

    What is the molar solubility of calcium oxalate calculated from a 0.0061-g residue?

    <p>$2.3 imes 10^{-9}$ M</p> Signup and view all the answers

    If 1.2 x $10^{-3}$ mol of lead(II) iodide dissolves in 1 L of solution, what does this information imply about its solubility product constant?

    <p>It is equal to 1.2 x $10^{-3}$ M</p> Signup and view all the answers

    Why might Ksp values not always be directly compared between different compounds?

    <p>Because they require a common dissociation stoichiometry</p> Signup and view all the answers

    In the context of solubility, what does the residue left after evaporation of a saturated solution represent?

    <p>The mass of solute that was originally dissolved</p> Signup and view all the answers

    What condition must be met for precipitation to occur in a solution?

    <p>The concentration of the ions must exceed Ksp.</p> Signup and view all the answers

    What does it mean if Q equals Ksp in a solution?

    <p>The solution is saturated.</p> Signup and view all the answers

    If the ion product Q is less than Ksp, what is the state of the solution?

    <p>The solution is unsaturated.</p> Signup and view all the answers

    What is the significance of the ion product in solubility reactions?

    <p>It represents the concentrations of the ions in the solution.</p> Signup and view all the answers

    What happens to a solution when Q is greater than Ksp?

    <p>Precipitation of the salt will occur.</p> Signup and view all the answers

    In a solubility reaction, what does the term Ksp represent?

    <p>The solubility product constant.</p> Signup and view all the answers

    If the concentrations of ions in a solution are equal to 0.15 M each, and Ksp is known to be $2.3 imes 10^{-9}$, what can be inferred?

    <p>It depends on the specific ionic compound.</p> Signup and view all the answers

    Why is the ion product referred to as the ion product instead of the reaction quotient?

    <p>Because it focuses on concentrations of ions only.</p> Signup and view all the answers

    What does the solubility product constant (Ksp) represent in the context of ionic compounds?

    <p>The equilibrium constant for the dissociation of a solid salt into its aqueous ions.</p> Signup and view all the answers

    In the dissociation reaction of a slightly soluble ionic compound M𝑝X𝑞, which expression represents the solubility product?

    <p>Ksp = [M𝑚+]^p[X𝑛−]^q</p> Signup and view all the answers

    When calculating molar solubility, what must be taken into account if the coefficients of the ions differ?

    <p>The molar solubility must be adjusted according to the coefficients.</p> Signup and view all the answers

    What relationship can be inferred if a compound is classified as insoluble in water?

    <p>It has a very low value of Ksp.</p> Signup and view all the answers

    Which of the following salts' dissociation expression corresponds to the Ksp: Ksp = [Ca][F]2?

    <p>CaF2</p> Signup and view all the answers

    What happens to the Ksp value as the solubility of a compound increases?

    <p>Ksp value increases.</p> Signup and view all the answers

    In the context of molar solubility, what does the term 'molar solubility' specifically refer to?

    <p>The number of moles of solute that will dissolve in one liter of solution.</p> Signup and view all the answers

    What does the notation M𝑝X𝑞 signify in a dissociation reaction?

    <p>The stoichiometry of the solid salt and its respective ions.</p> Signup and view all the answers

    What happens to the solubility of insoluble ionic hydroxides as the pH increases?

    <p>Solubility decreases</p> Signup and view all the answers

    Which statement describes selective precipitation?

    <p>It separates ions by forming insoluble salts with different solubility products.</p> Signup and view all the answers

    How does lowering the pH affect the solubility of ionic compounds containing anions of weak acids?

    <p>Solubility increases</p> Signup and view all the answers

    In fractional precipitation, what is essential for a reagent to be effective?

    <p>It must form an insoluble salt with cations of differing Ksp values.</p> Signup and view all the answers

    Which of the following statements is true about the relationship between pH and ion concentration in a solution containing ionic hydroxides?

    <p>A higher pH decreases the solubility leading to fewer Mn+ ions.</p> Signup and view all the answers

    What is the effect of adding H3O+ to a solution containing carbonate ions (CO32−)?

    <p>It increases the solubility of carbonate compounds.</p> Signup and view all the answers

    Study Notes

    Solubility Equilibria

    • All ionic compounds dissolve in water to some degree, but many have low solubility and are classified as insoluble.
    • The equilibrium constant Ksp can be used to determine the relative solubilities of salts in water.

    Solubility Product Constant (Ksp)

    • Ksp is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly insoluble) ionic compound.
    • It represents the dissociation of a solid salt into its aqueous ions.
    • The solubility product expression is: Ksp = [Mm+]p [Xn−]q

    Molar Solubility (s)

    • Molar solubility is the number of moles of solute that will dissolve in a liter of solution.
    • It is related to Ksp and represents the molarity of the dissolved solute in a saturated solution.
    • Ksp values of compounds cannot always be compared, and the compounds must have the same dissociation stoichiometry.

    Example Calculations

    • Calculate the molar solubility of CaC2O4 given Ksp and residue mass.
    • Calculate the solubility product constant of PbI2 given experimental data.

    Solubility and the Common-Ion Effect

    • Addition of a soluble salt that contains one of the ions of the slightly soluble salt decreases the solubility of the slightly soluble salt.
    • This is because the added ion shifts the equilibrium to the left.

    Precipitation

    • Precipitation occurs when the concentrations of the ions exceed the solubility of the ionic compound.
    • Compare the ion product, Q, to Ksp to determine if precipitation will occur:
      • Q = Ksp: saturated solution, no precipitation.
      • Q < Ksp: unsaturated solution, no precipitation.
      • Q > Ksp: supersaturated solution, precipitation will occur.

    Fractional Precipitation

    • This technique is used to separate two or more ions from a solution by adding a reactant that precipitates first one ion, then another.
    • A successful reagent can precipitate with more than one cation if their Ksp values are significantly different.

    Effect of pH on Solubility

    • For insoluble ionic hydroxides, higher pH decreases solubility, and lower pH increases solubility.
    • For insoluble ionic compounds containing anions of weak acids, lower pH increases solubility.

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    Related Documents

    Chapter 15: Equilibria PDF

    Description

    Understanding solubility of ionic compounds in water and the solubility product constant (Ksp) that determines their relative solubilities.

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