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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?
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?
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?
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?
What is the solubility product for calcium oxalate?
What is the effect of the common-ion effect on the solubility product of the slightly soluble salt?
What is the effect of the common-ion effect on the solubility product of the slightly soluble salt?
Why does the addition of Pb(NO3)2 to the solubility equilibrium of solid PbCrO4 decrease the solubility of PbCrO4?
Why does the addition of Pb(NO3)2 to the solubility equilibrium of solid PbCrO4 decrease the solubility of PbCrO4?
What is the purpose of calculating the molar solubility of a slightly soluble salt?
What is the purpose of calculating the molar solubility of a slightly soluble salt?
What is the condition necessary for the common-ion effect to occur?
What is the condition necessary for the common-ion effect to occur?
What is molar solubility in the context of a saturated solution?
What is molar solubility in the context of a saturated solution?
Under what condition can the Ksp values of different compounds be meaningfully compared?
Under what condition can the Ksp values of different compounds be meaningfully compared?
What does the Ksp represent for a compound like calcium oxalate in a saturated solution?
What does the Ksp represent for a compound like calcium oxalate in a saturated solution?
If a saturated solution of calcium oxalate produces a residue of 0.0061 g after evaporation, what information can be calculated?
If a saturated solution of calcium oxalate produces a residue of 0.0061 g after evaporation, what information can be calculated?
What is the molar solubility of calcium oxalate calculated from a 0.0061-g residue?
What is the molar solubility of calcium oxalate calculated from a 0.0061-g residue?
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?
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?
Why might Ksp values not always be directly compared between different compounds?
Why might Ksp values not always be directly compared between different compounds?
In the context of solubility, what does the residue left after evaporation of a saturated solution represent?
In the context of solubility, what does the residue left after evaporation of a saturated solution represent?
What condition must be met for precipitation to occur in a solution?
What condition must be met for precipitation to occur in a solution?
What does it mean if Q equals Ksp in a solution?
What does it mean if Q equals Ksp in a solution?
If the ion product Q is less than Ksp, what is the state of the solution?
If the ion product Q is less than Ksp, what is the state of the solution?
What is the significance of the ion product in solubility reactions?
What is the significance of the ion product in solubility reactions?
What happens to a solution when Q is greater than Ksp?
What happens to a solution when Q is greater than Ksp?
In a solubility reaction, what does the term Ksp represent?
In a solubility reaction, what does the term Ksp represent?
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?
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?
Why is the ion product referred to as the ion product instead of the reaction quotient?
Why is the ion product referred to as the ion product instead of the reaction quotient?
What does the solubility product constant (Ksp) represent in the context of ionic compounds?
What does the solubility product constant (Ksp) represent in the context of ionic compounds?
In the dissociation reaction of a slightly soluble ionic compound M𝑝X𝑞, which expression represents the solubility product?
In the dissociation reaction of a slightly soluble ionic compound M𝑝X𝑞, which expression represents the solubility product?
When calculating molar solubility, what must be taken into account if the coefficients of the ions differ?
When calculating molar solubility, what must be taken into account if the coefficients of the ions differ?
What relationship can be inferred if a compound is classified as insoluble in water?
What relationship can be inferred if a compound is classified as insoluble in water?
Which of the following salts' dissociation expression corresponds to the Ksp: Ksp = [Ca][F]2?
Which of the following salts' dissociation expression corresponds to the Ksp: Ksp = [Ca][F]2?
What happens to the Ksp value as the solubility of a compound increases?
What happens to the Ksp value as the solubility of a compound increases?
In the context of molar solubility, what does the term 'molar solubility' specifically refer to?
In the context of molar solubility, what does the term 'molar solubility' specifically refer to?
What does the notation M𝑝X𝑞 signify in a dissociation reaction?
What does the notation M𝑝X𝑞 signify in a dissociation reaction?
What happens to the solubility of insoluble ionic hydroxides as the pH increases?
What happens to the solubility of insoluble ionic hydroxides as the pH increases?
Which statement describes selective precipitation?
Which statement describes selective precipitation?
How does lowering the pH affect the solubility of ionic compounds containing anions of weak acids?
How does lowering the pH affect the solubility of ionic compounds containing anions of weak acids?
In fractional precipitation, what is essential for a reagent to be effective?
In fractional precipitation, what is essential for a reagent to be effective?
Which of the following statements is true about the relationship between pH and ion concentration in a solution containing ionic hydroxides?
Which of the following statements is true about the relationship between pH and ion concentration in a solution containing ionic hydroxides?
What is the effect of adding H3O+ to a solution containing carbonate ions (CO32−)?
What is the effect of adding H3O+ to a solution containing carbonate ions (CO32−)?
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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Description
Understanding solubility of ionic compounds in water and the solubility product constant (Ksp) that determines their relative solubilities.
