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Questions and Answers
What is the formula to calculate pH from pOH?
What is the formula to calculate pH from pOH?
- pH = pOH / 14
- pH = pOH + 14
- pH = 14 - pOH (correct)
- pH = 14 * pOH
Which components are essential for a solution to act as a buffer?
Which components are essential for a solution to act as a buffer?
- A weak base and its conjugate acid (correct)
- A strong acid and its conjugate base
- A strong base and its conjugate acid
- A weak acid and its conjugate base (correct)
What does buffer capacity refer to?
What does buffer capacity refer to?
- The physical state of the buffer in the solution
- The total volume of a buffer solution
- The amount of acid or base a buffer can neutralize without significant pH change (correct)
- The ability of a buffer to resist pH changes with high temperatures
How can pH be calculated for a buffer solution using the Henderson-Hasselbalch equation?
How can pH be calculated for a buffer solution using the Henderson-Hasselbalch equation?
What is the optimal pH range for a buffer to effectively resist pH changes?
What is the optimal pH range for a buffer to effectively resist pH changes?
Which statement accurately describes the Arrhenius Theory of acids and bases?
Which statement accurately describes the Arrhenius Theory of acids and bases?
What is the relationship between solubility and the solubility product constant (Ksp)?
What is the relationship between solubility and the solubility product constant (Ksp)?
Which best describes the Common Ion Effect?
Which best describes the Common Ion Effect?
What is pH defined as?
What is pH defined as?
How do you calculate the solubility of a salt from its Ksp value?
How do you calculate the solubility of a salt from its Ksp value?
Which of the following correctly defines a weak acid in relation to pH calculations?
Which of the following correctly defines a weak acid in relation to pH calculations?
What distinguishes the Brønsted-Lowry theory from the Arrhenius theory?
What distinguishes the Brønsted-Lowry theory from the Arrhenius theory?
Which statement is true regarding the Lewis Theory of acids and bases?
Which statement is true regarding the Lewis Theory of acids and bases?
Flashcards
Arrhenius Theory
Arrhenius Theory
Acids produce H+ ions in aqueous solutions, while bases produce OH- ions.
Brønsted-Lowry Theory
Brønsted-Lowry Theory
An acid is a proton (H+) donor and a base is a proton acceptor.
Lewis Theory
Lewis Theory
An acid is an electron pair acceptor, and a base is an electron pair donor.
Solubility Equilibrium
Solubility Equilibrium
Dynamic equilibrium between a solid and its dissolved ions in a saturated solution.
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Solubility Product Constant (Ksp)
Solubility Product Constant (Ksp)
A constant for a sparingly soluble salt at a given temperature representing the equilibrium between the solid and its ions..
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Common Ion Effect
Common Ion Effect
Solubility of a sparingly soluble salt decreases when a soluble salt with a common ion is added.
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pH
pH
pH = -log[H+]
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pH Calculation (Strong Acids)
pH Calculation (Strong Acids)
Direct calculation using the concentration of H+ ions.
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pH Calculation (Weak Acids)
pH Calculation (Weak Acids)
Calculation based on Ka (acid dissociation constant) and initial concentration using ICE table.
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pH of Strong Bases
pH of Strong Bases
Calculate pOH from [OH-], then use pH + pOH = 14 to find pH.
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Weak Bases Calculations
Weak Bases Calculations
Use approximations to find ion concentrations in equilibrium equations.
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pH and pOH
pH and pOH
Inverse relationship in water; pH + pOH = 14
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Buffer Solution
Buffer Solution
Resists pH change with acid/base addition.
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Buffer Components
Buffer Components
Weak acid + conjugate base (or weak base + conjugate acid).
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Buffer Action
Buffer Action
Weak acid/base neutralize added H+/OH- ions
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Henderson-Hasselbalch Equation
Henderson-Hasselbalch Equation
pH = pKa + log ([conjugate base]/[weak acid])
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Buffer Capacity
Buffer Capacity
Amount of acid/base a buffer neutralizes before pH changes.
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Buffer Range
Buffer Range
pH range where buffer effectively resists change.
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Calculating pH from pOH
- pH + pOH = 14
Buffer Components
- A weak acid and its conjugate base
- Or a weak base and its conjugate acid
Buffer Capacity
- The amount of acid or base a buffer can neutralize before a significant change in pH occurs
Henderson-Hasselbalch Equation
- pH = pKa + log([A-]/[HA])
- Where:
- pKa: The negative logarithm of the acid dissociation constant (Ka)
- [A-]: The concentration of the conjugate base
- [HA]: The concentration of the weak acid
Optimal Buffer pH Range
- A buffer works best within ± 1 pH unit of its pKa
Arrhenius Theory of Acids and Bases
- Acids produce hydrogen ions (H+) in water, and bases produce hydroxide ions (OH-) in water
Solubility & Ksp Relationship
- Ksp is the product of the ion concentrations at equilibrium in a saturated solution
- A higher Ksp value indicates greater solubility
Common Ion Effect
- The solubility of a sparingly soluble salt decreases when a soluble compound containing a common ion is added to the solution
pH Definition
- pH is the negative logarithm of the hydrogen ion concentration ([H+]) in a solution
Calculating Salt Solubility from Ksp
- Use the equilibrium constant expression for the dissolution of the salt and solve for the solubility of the salt
Weak Acid Definition
- A weak acid ionizes only partially in solution, resulting in a pH higher than that of a strong acid at the same concentration
Brønsted-Lowry vs. Arrhenius Theory
- Brønsted-Lowry theory defines acids as proton donors (H+) and bases as proton acceptors, whereas Arrhenius theory focuses on the production of H+ or OH- in aqueous solutions
Lewis Theory of Acids and Bases
- Lewis acids accept electron pairs, and Lewis bases donate electron pairs. This definition encompasses both proton-based interactions and electron-pair sharing interactions.
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