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Questions and Answers
What distinguishes a strong acid from a weak acid according to the Bronsted-Lowry definition?
What distinguishes a strong acid from a weak acid according to the Bronsted-Lowry definition?
- Strong acids can only react with bases, while weak acids can react with both bases and other acids.
- Strong acids only donate protons, while weak acids accept protons.
- Strong acids completely dissociate in solution while weak acids do not. (correct)
- Strong acids have higher molecular weights than weak acids.
In the acid-dissociation equation HA ⇌ H⁺ + A⁻, which species is considered the conjugate base?
In the acid-dissociation equation HA ⇌ H⁺ + A⁻, which species is considered the conjugate base?
- Both A⁻ and H⁺
- A⁻ (correct)
- HA
- H⁺
How does the equilibrium constant (Ka) relate to the strength of an acid?
How does the equilibrium constant (Ka) relate to the strength of an acid?
- Ka is related solely to the molecular structure of the acid.
- Stronger acids have higher Ka values. (correct)
- Ka values do not affect acid strength.
- Higher Ka values indicate weaker acids.
At what point on the titration curve does the pKa of an acid correspond?
At what point on the titration curve does the pKa of an acid correspond?
How does the ratio of [HA] to [A⁻] change with increasing pH?
How does the ratio of [HA] to [A⁻] change with increasing pH?
Flashcards
Brønsted-Lowry acid/base
Brønsted-Lowry acid/base
An acid is a proton donor, and a base is a proton acceptor.
Acid strength (strong vs. weak)
Acid strength (strong vs. weak)
Strong acids completely dissociate in water, while weak acids only partially dissociate.
Acid dissociation equation
Acid dissociation equation
Represents the breakdown of an acid into ions (proton and conjugate base).
pKa and Ka
pKa and Ka
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Henderson-Hasselbalch equation
Henderson-Hasselbalch equation
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Study Notes
Brønsted-Lowry Acid-Base Definitions
- A Brønsted-Lowry acid is a proton (H+) donor.
- A Brønsted-Lowry base is a proton acceptor.
Acid Strength
- Strong acids completely dissociate in water.
- Weak acids only partially dissociate in water.
Acid-Dissociation Equations
- Acid-dissociation equations show the equilibrium between an acid and its conjugate base in water.
- Example: HA + H₂O ⇌ H₃O⁺ + A⁻
- HA is the acid.
- A⁻ is the conjugate base.
Equilibrium Constant (Ka) and pKa
- Ka is the acid dissociation constant, quantifying the strength of an acid.
- Larger Ka values indicate stronger acids.
- pKa = -log₁₀Ka; lower pKa values correspond to stronger acids.
Titration Curves and pKa
- pKa is found at the midpoint of the titration curve's buffer region.
- This is where the concentrations of the acid (HA) and conjugate base (A⁻) are equal.
[HA]:[A⁻] and pH
- The ratio of [HA] to [A⁻] changes with pH.
Henderson-Hasselbalch Equation
- The Henderson-Hasselbalch equation relates pKa, pH, and the ratio of [HA] to [A⁻].
- It allows calculation of the ratio of [HA] to [A⁻] at a given pH.
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