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Questions and Answers
How does the addition of a common ion affect the equilibrium of a solution, according to Le Chatelier's Principle?
How does the addition of a common ion affect the equilibrium of a solution, according to Le Chatelier's Principle?
- It causes the reaction to shift towards the reactants, reducing the solubility or ionization of the original substance. (correct)
- It has no effect on the equilibrium as the common ion is already present.
- It initially shifts the reaction towards the products, but eventually shifts back to the reactants.
- It causes the reaction to shift towards the products, increasing the solubility of the original substance.
A solution contains both a weak acid and its conjugate base. How does this solution resist changes in pH when a strong acid is added?
A solution contains both a weak acid and its conjugate base. How does this solution resist changes in pH when a strong acid is added?
- The conjugate base in the solution reacts with the added acid, neutralizing it. (correct)
- The strong acid reacts with water, neutralizing its effect on pH.
- The strong acid is buffered by the inert ions present in the solution.
- The weak acid in the solution reacts with the added acid, neutralizing it.
Why can a mixture of hydrofluoric acid (HF) and sodium fluoride (NaF) act as a buffer solution?
Why can a mixture of hydrofluoric acid (HF) and sodium fluoride (NaF) act as a buffer solution?
- HF and NaF do not form a buffer solution because they are not a conjugate acid-base pair.
- HF is a strong acid and NaF is a strong base.
- HF is a weak acid that neutralizes added bases, and fluoride ion (F-) from NaF neutralizes added acids. (correct)
- HF is a weak acid that neutralizes added acids, and fluoride ion (F-) from NaF neutralizes added bases.
Ammonia (NH3) can react with hydrochloric acid (HCl) to create a buffer. What are the roles of NH3 and the resulting product in this buffer system?
Ammonia (NH3) can react with hydrochloric acid (HCl) to create a buffer. What are the roles of NH3 and the resulting product in this buffer system?
What is the primary purpose of the Henderson-Hasselbalch equation?
What is the primary purpose of the Henderson-Hasselbalch equation?
In an acid-base titration, what is the 'equivalence point'?
In an acid-base titration, what is the 'equivalence point'?
During a titration, an indicator changes color, signaling that the titration is complete. What is the correct term for this?
During a titration, an indicator changes color, signaling that the titration is complete. What is the correct term for this?
What is the purpose of using a reaction table with moles (or mmol) during a titration, as opposed to a table with molarity (or mM)?
What is the purpose of using a reaction table with moles (or mmol) during a titration, as opposed to a table with molarity (or mM)?
What information does the solubility product constant, Ksp, provide about a compound?
What information does the solubility product constant, Ksp, provide about a compound?
How is molar solubility defined?
How is molar solubility defined?
If you are given the molar solubility (s) of a salt, how can you calculate the solubility product constant (Ksp) of the salt?
If you are given the molar solubility (s) of a salt, how can you calculate the solubility product constant (Ksp) of the salt?
How does the presence of a common ion generally affect the solubility of a salt?
How does the presence of a common ion generally affect the solubility of a salt?
What is the effect of increasing temperature on the solubility of a salt in water?
What is the effect of increasing temperature on the solubility of a salt in water?
How does a change in pH affect the solubility of salts that contain ions which are conjugate acids or bases of weak substances?
How does a change in pH affect the solubility of salts that contain ions which are conjugate acids or bases of weak substances?
When does precipitation occur in a solution, and how does the reaction quotient, Q, relate to this?
When does precipitation occur in a solution, and how does the reaction quotient, Q, relate to this?
What is the common ion effect?
What is the common ion effect?
Which of the following best describes a buffer solution?
Which of the following best describes a buffer solution?
Why is a mixture of a weak acid and its conjugate base able to act as a buffer?
Why is a mixture of a weak acid and its conjugate base able to act as a buffer?
What is the process of titration used for?
What is the process of titration used for?
Which of the following best describes the 'titrant' in a titration?
Which of the following best describes the 'titrant' in a titration?
What is indicated by the 'end point' in a titration?
What is indicated by the 'end point' in a titration?
What is the role of an indicator in a titration?
What is the role of an indicator in a titration?
In what situation is it most appropriate to use a reaction table constructed with molarities to calculate pH at a point in a titration?
In what situation is it most appropriate to use a reaction table constructed with molarities to calculate pH at a point in a titration?
What does the solubility product constant, Ksp, represent?
What does the solubility product constant, Ksp, represent?
Which of the following correctly describes the relationship between Ksp and molar solubility?
Which of the following correctly describes the relationship between Ksp and molar solubility?
What is the effect of temperature on the solubility of a salt?
What is the effect of temperature on the solubility of a salt?
How might the pH of a solution affect the solubility of a slightly soluble salt?
How might the pH of a solution affect the solubility of a slightly soluble salt?
Under what condition will precipitation occur in a solution?
Under what condition will precipitation occur in a solution?
How does the addition of a common ion impact the solubility of a sparingly soluble salt?
How does the addition of a common ion impact the solubility of a sparingly soluble salt?
What is the defining characteristic of a buffer solution?
What is the defining characteristic of a buffer solution?
Which component of a buffer solution neutralizes added acids?
Which component of a buffer solution neutralizes added acids?
What is the primary purpose of performing a titration?
What is the primary purpose of performing a titration?
What term describes the solution of known concentration used in a titration?
What term describes the solution of known concentration used in a titration?
In a titration, what signifies the 'end point'?
In a titration, what signifies the 'end point'?
What is the role of the indicator used in a titration experiment?
What is the role of the indicator used in a titration experiment?
Which of the following situations requires the use of a reaction table with molarities, rather than moles, to calculate pH during a titration?
Which of the following situations requires the use of a reaction table with molarities, rather than moles, to calculate pH during a titration?
What information does the solubility product constant, Ksp, directly provide?
What information does the solubility product constant, Ksp, directly provide?
How can you determine the Ksp value if you know the molar solubility of a compound?
How can you determine the Ksp value if you know the molar solubility of a compound?
What effect does increasing the temperature typically have on the solubility of a salt in water?
What effect does increasing the temperature typically have on the solubility of a salt in water?
How can pH affect the solubility of a salt in an aqueous solution?
How can pH affect the solubility of a salt in an aqueous solution?
Under what condition will precipitation occur in a solution according to the reaction quotient (Q)?
Under what condition will precipitation occur in a solution according to the reaction quotient (Q)?
Flashcards
Common Ion Effect
Common Ion Effect
When a solution has two substances sharing a common ion, it reduces solubility/ionization. Adding more product shifts the reaction towards reactants (Le Chatelier's Principle).
Buffer Solution
Buffer Solution
A solution that resists pH changes with small acid/base additions. Contains an acid and conjugate base (or vice versa).
HF and NaF as a Buffer
HF and NaF as a Buffer
HF is a weak acid; NaF provides F- (conjugate base). HF neutralizes added bases, F- neutralizes acids, stabilizing pH.
NH3 and HCl as a Buffer
NH3 and HCl as a Buffer
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Henderson-Hasselbalch Equation
Henderson-Hasselbalch Equation
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Titration
Titration
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Titrant
Titrant
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Equivalence Point
Equivalence Point
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End Point
End Point
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Indicator
Indicator
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Solubility Product Constant (Ksp)
Solubility Product Constant (Ksp)
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Molar Solubility
Molar Solubility
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Common Ion Effect on Solubility
Common Ion Effect on Solubility
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Factors Affecting Solubility
Factors Affecting Solubility
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Precipitation Conditions
Precipitation Conditions
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Study Notes
Common Ion Effect
- A solution with two substances sharing a common ion experiences this effect
- Presence of a common ion reduces solubility or ionization of one of the substances
- Le Chatelier's Principle states adding more product (common ion) shifts reaction to reactants' side
- Introducing NaF to HF causes it to break apart, adding F- to the solution, shifting the reaction to the left
Buffer Solutions
- Buffer solutions resist pH changes upon addition of small amounts of acids or bases
- Buffers contain both an acid and its conjugate base, or a base and its conjugate acid
- The base component neutralizes added acid
- The acid component neutralizes added base
HF and NaF as a Buffer
- HF, a weak acid, and NaF, its conjugate base, combine to form a buffer solution
- HF neutralizes added bases
- F- neutralizes added acids
- Together, they stabilize the pH of the solution
NH3 and HCl as a Buffer
- Ammonia (NH3) is a weak base
- HCl reacting with NH3 forms NH4+, the conjugate acid
- This combination works as a buffer
- NH3 can react with added acids successfully
- NH4+ can react with added bases successfully
Henderson-Hasselbalch Equation
- This equation calculates the pH of a buffer
- Moles of conjugate acid and base after adding strong acid/base are determined
- Concentrations are calculated and put in an ICE table
- Solving the ICE table allows calculation of pH using E concentrations
- The Henderson-Hasselbalch equation offers a faster method
Titration Definitions
- Titration: A lab technique to find the concentration of a substance by adding one solution slowly to another until the reaction is complete
- Titrant: The solution added from a burette in a titration
- Equivalence Point: The point the acid equals the base in a titration, meaning the reaction is complete
- End Point: The point where the indicator changes color, showing the titration is complete, close to the equivalence point if the correct indicator is chosen.
- Indicator: A substance that changes color at a certain pH to show the end of a titration
Titration Curve Sketches
- Strong acid, strong base titrations: Refer to figure 17.3
- Weak acid, strong base titrations: Refer to figure 17.4
- Strong acid, weak base titrations: Refer to figure 17.6
Reaction Tables
- Use an ICE table with molarities for a solution with only a weak base or weak acid
- Use an ICE table with molarities before adding any titrant and at the equivalence point
- Use a table in units of moles at every other point in the titration where you a mixture of a weak acid/base and a strong base/acid
Solubility Product Constant
- Ksp represents a compound's solubility in water
- Ksp equals the product of ion concentrations in a saturated solution
- Each concentration is raised to the power of its coefficient from the balanced equation
Molar Solubility
- The number of moles of a compound that can dissolve in 1 liter of water before saturation
Ksp and Molar Solubility Relation
- Use an ICE table to calculate solubility and Ksp
- Molar solubility is ‘x’ in the ICE table for calculating Ksp
- If given Ksp, use the ICE table to solve for 'x' to find molar solubility
Common Ion Effect on Salt Solubility
- The common ion effect reduces the solubility of a salt
- Reduced solubility occurs because the solution can't hold the same ion
- Reactant-side equilibrium shift (undissolved salt) occurs because of the addition of the ion
Factors Affecting Salt Solubility
- Higher temperatures usually increase solubility
- Changes in pH can alter solubility based on the salt's acidic or basic ions
- Increased pH will cause the equilibrium to shift towards the reactants and increase the CN⁻ in solution
- Decreased pH decreases the amount of OH- which decreases the amount of CN- in solution, increasing the solubility of AgCN.
Conditions for Precipitation
- Precipitation occurs when the ion concentration product surpasses Ksp
- Solutions with excessive ions form precipitates
- The Q determines if precipitation will occur
- A precipitate forms when Q > Ksp
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Description
Learn about the common ion effect and buffer solutions. The common ion effect occurs when a solution contains two substances that share a common ion, reducing solubility or ionization. Buffer solutions resist pH changes by containing an acid and its conjugate base, or a base and its conjugate acid.
