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Questions and Answers
What is the effect of adding a common ion to a saturated solution of a slightly soluble salt?
What is the effect of adding a common ion to a saturated solution of a slightly soluble salt?
What is the principle that explains the common ion effect?
What is the principle that explains the common ion effect?
How does the common ion effect influence the solubility product constant (Ksp)?
How does the common ion effect influence the solubility product constant (Ksp)?
Which of the following scenarios would demonstrate the common ion effect?
Which of the following scenarios would demonstrate the common ion effect?
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Consider a saturated solution of lead(II) chloride (PbCl2). Adding a common ion would result in:
Consider a saturated solution of lead(II) chloride (PbCl2). Adding a common ion would result in:
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In a saturated solution of silver chloride (AgCl), what happens to the solubility of AgCl when a soluble chloride salt like NaCl is added?
In a saturated solution of silver chloride (AgCl), what happens to the solubility of AgCl when a soluble chloride salt like NaCl is added?
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Which of the following expressions correctly represents the solubility product constant (Ksp) for PbCl2?
Which of the following expressions correctly represents the solubility product constant (Ksp) for PbCl2?
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What is the effect of adding a common ion to a saturated solution of a slightly soluble salt on the reaction quotient (Qsp)?
What is the effect of adding a common ion to a saturated solution of a slightly soluble salt on the reaction quotient (Qsp)?
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Which of the following statements accurately describes the common ion effect?
Which of the following statements accurately describes the common ion effect?
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In a saturated solution of CaF2, the addition of which of the following will cause the solubility of CaF2 to decrease?
In a saturated solution of CaF2, the addition of which of the following will cause the solubility of CaF2 to decrease?
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When a common ion is added to a saturated solution of a slightly soluble salt, the solubility of the salt:
When a common ion is added to a saturated solution of a slightly soluble salt, the solubility of the salt:
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Which of the following accurately describes the role of Le Chatelier's principle in the common ion effect?
Which of the following accurately describes the role of Le Chatelier's principle in the common ion effect?
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What is the relationship between the reaction quotient (Qsp) and the solubility product constant (Ksp) when a common ion is added to a saturated solution of a slightly soluble salt?
What is the relationship between the reaction quotient (Qsp) and the solubility product constant (Ksp) when a common ion is added to a saturated solution of a slightly soluble salt?
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Which of the following statements about the Ksp of a slightly soluble salt is TRUE?
Which of the following statements about the Ksp of a slightly soluble salt is TRUE?
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In an ICE table used to calculate the molar solubility of a slightly soluble salt in the presence of a common ion, the 'Change' row represents:
In an ICE table used to calculate the molar solubility of a slightly soluble salt in the presence of a common ion, the 'Change' row represents:
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The approximation used in calculations involving the common ion effect is valid when:
The approximation used in calculations involving the common ion effect is valid when:
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Which of the following scenarios would NOT illustrate the common ion effect?
Which of the following scenarios would NOT illustrate the common ion effect?
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A saturated solution of silver chloride (AgCl) is in equilibrium with Ag+ and Cl- ions. What happens to the solubility of AgCl when a small amount of sodium chloride (NaCl) is added?
A saturated solution of silver chloride (AgCl) is in equilibrium with Ag+ and Cl- ions. What happens to the solubility of AgCl when a small amount of sodium chloride (NaCl) is added?
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Flashcards
Common Ion Effect
Common Ion Effect
The decrease in solubility of a salt due to the presence of a common ion.
Le Chatelier's Principle
Le Chatelier's Principle
If an equilibrium system is disturbed, it will shift to counteract the disturbance.
Qsp
Qsp
The reaction quotient for a salt's solubility which indicates the current state of equilibrium.
Ksp
Ksp
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ICE Table
ICE Table
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Effect of Common Ion
Effect of Common Ion
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Common Ion Concentration
Common Ion Concentration
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Molar Solubility in KCl
Molar Solubility in KCl
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Qsp and Ksp Relation
Qsp and Ksp Relation
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Solubility of PbCl2
Solubility of PbCl2
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Impact of KCl on PbCl2
Impact of KCl on PbCl2
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Direction of Solubility Shift
Direction of Solubility Shift
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Chemical Equilibrium Concept
Chemical Equilibrium Concept
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Understanding Qsp vs Ksp
Understanding Qsp vs Ksp
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Effect of Common Ion on Solubility
Effect of Common Ion on Solubility
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Understanding Ksp Stability
Understanding Ksp Stability
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Using ICE Table for Solubility
Using ICE Table for Solubility
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Study Notes
Common Ion Effect
- The presence of a common ion decreases the solubility of a slightly soluble salt.
- A saturated solution of lead(II) chloride (PbCl₂) is at equilibrium, with dissolved Pb²⁺ and Cl⁻ ions. The mole ratio is 1:2 (Pb²⁺ : Cl⁻).
- Adding a soluble salt containing a common ion (like KCl) disrupts the equilibrium.
- The addition of chloride ions (Cl⁻) from KCl shifts the system to the left, per Le Chatelier's Principle, decreasing the concentration of lead(II) and chloride ions to relieve the stress of increased chloride ion concentration.
- This results in more solid PbCl₂ forming, lowering PbCl₂ solubility.
- The common ion effect is the decrease in the solubility of a sparingly soluble salt in the presence of a common ion.
- The presence of a common ion affects the molar solubility of lead(II) chloride.
- A saturated solution of lead(II) chloride is at equilibrium, where the rate of dissolution equals the rate of precipitation, and the ion concentration remains constant.
- Adding a common ion, such as chloride ions from potassium chloride (KCl), increases the chloride ion concentration, disrupting this equilibrium.
- This shift results in lead(II) ions combining with chloride ions, fostering further lead(II) chloride precipitation.
- The common ion effect is demonstrable using the reaction quotient (Qsp). When Ksp = Qsp, the system is at equilibrium. A common ion increases Qsp, causing a shift to the left, reducing Qsp until it equals Ksp.
- Qsp is a measure of the relative amounts of products and reactants at any given time.
- Qsp > Ksp: The system is not at equilibrium, and the reaction will shift to the left (toward reactants);
- Qsp < Ksp: The system is not at equilibrium, and the reaction will shift to the right (toward products);
- Qsp = Ksp: The system is at equilibrium.
- Ksp is a constant that represents the product of the ion concentrations raised to their stoichiometric coefficients in a saturated solution at a given temperature. Ksp is a constant for a given compound at a specific temperature; it does not change with the addition of a common ion.
Using the Reaction Quotient (Qsp)
- At equilibrium, the reaction quotient (Qsp) equals the solubility product constant (Ksp).
- Adding a common ion increases Qsp, making it greater than Ksp, so the system is no longer at equilibrium.
- The system shifts left to decrease Qsp until it equals Ksp.
Quantifying the Common Ion Effect
- The molar solubility of PbCl₂ can be calculated using an ICE table in a solution containing 0.10 M KCl.
- The presence of the common ion (Cl⁻) from KCl reduces the molar solubility of PbCl₂.
- The molar solubility of PbCl₂ in 0.10 M KCl is significantly lower than its molar solubility in pure water.
- The Ksp value for PbCl₂ remains constant at a given temperature, but the molar solubility decreases due to the common ion effect.
- In a pure lead(II) chloride solution, the molar solubility is 0.016 M at 25°C.
- In a 0.10 M potassium chloride solution, the molar solubility of lead(II) chloride drops to 0.0017 M at 25°C.
- An ICE (Initial, Change, Equilibrium) table can be used to calculate the molar solubility of a slightly soluble salt in the presence of a common ion,.
- In the presence of a common ion, the change in concentration (X) is often negligible compared to the initial concentration of the common ion, simplifying calculations.
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Description
Explore the common ion effect and its impact on solubility equilibria in lead(II) chloride. Understand how the addition of a common ion like chloride ions influences the dissolution and precipitation processes according to Le Chatelier's principle.
