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Questions and Answers
What characterizes an Arrhenius acid?
What characterizes an Arrhenius acid?
- It produces hydrogen ions in solution. (correct)
- It is a molecular compound that does not ionize.
- It produces hydroxide ions in solution.
- It donates a hydrogen ion to another substance.
How does an Arrhenius base differ from an Arrhenius acid?
How does an Arrhenius base differ from an Arrhenius acid?
- An Arrhenius base accepts hydrogen ions; an acid does not.
- An Arrhenius base produces hydrogen ions; an acid does not.
- An Arrhenius base does not dissociate in water.
- An Arrhenius base produces hydroxide ions; an acid does not. (correct)
What is ionization according to Arrhenius theory?
What is ionization according to Arrhenius theory?
- Production of only positive ions from a compound.
- Release of ions from an ionic compound.
- Production of individual ions from a dissolved molecular compound. (correct)
- Formation of hydrogen ions from water.
What process is described as dissociation in the context of Arrhenius bases?
What process is described as dissociation in the context of Arrhenius bases?
Which of the following statements is true regarding an Arrhenius acid?
Which of the following statements is true regarding an Arrhenius acid?
Which option describes the overall role of an Arrhenius base in a neutralization reaction?
Which option describes the overall role of an Arrhenius base in a neutralization reaction?
In the context of Arrhenius theory, what makes acids and bases unique?
In the context of Arrhenius theory, what makes acids and bases unique?
What defines the ionization process in Arrhenius acids?
What defines the ionization process in Arrhenius acids?
Which statement correctly defines an acid and a base?
Which statement correctly defines an acid and a base?
In the Brønsted–Lowry acid-base theory, what happens in the reaction HF(aq) + H2O(l) ⇌ H3O+(aq) + F–(aq)?
In the Brønsted–Lowry acid-base theory, what happens in the reaction HF(aq) + H2O(l) ⇌ H3O+(aq) + F–(aq)?
Which of the following is an example of an amphiprotic substance?
Which of the following is an example of an amphiprotic substance?
What characterizes a monoprotic acid?
What characterizes a monoprotic acid?
Which of the following pairs represents a conjugate acid-base pair in the given reaction: HF(aq) + H2O(l) ⇌ H3O+(aq) + F–(aq)?
Which of the following pairs represents a conjugate acid-base pair in the given reaction: HF(aq) + H2O(l) ⇌ H3O+(aq) + F–(aq)?
What is the role of a base in an acid-base reaction according to the Brønsted–Lowry theory?
What is the role of a base in an acid-base reaction according to the Brønsted–Lowry theory?
During the dissociation of a diprotic acid, what can be inferred if one mole of the acid can donate two protons?
During the dissociation of a diprotic acid, what can be inferred if one mole of the acid can donate two protons?
Which of the following identifies a fundamental property of acids in water?
Which of the following identifies a fundamental property of acids in water?
What is the pKa of a solution with a Ka of 6.3 x 10–4?
What is the pKa of a solution with a Ka of 6.3 x 10–4?
Which statement correctly describes the nature of buffers?
Which statement correctly describes the nature of buffers?
What happens when a base is added to a buffer solution?
What happens when a base is added to a buffer solution?
What is a major component of a buffer system?
What is a major component of a buffer system?
What occurs when excess H3O+ ions are introduced to a buffer solution?
What occurs when excess H3O+ ions are introduced to a buffer solution?
Which of the following best describes a buffer's ability to respond to added acid or base?
Which of the following best describes a buffer's ability to respond to added acid or base?
Which active species in a buffer reacts with added acids?
Which active species in a buffer reacts with added acids?
What is the primary function of a buffer solution in a chemical context?
What is the primary function of a buffer solution in a chemical context?
What characterizes a diprotic acid?
What characterizes a diprotic acid?
Which statement is true regarding triprotic acids?
Which statement is true regarding triprotic acids?
How are polyprotic acids defined?
How are polyprotic acids defined?
What distinguishes a monoprotic acid from diprotic and triprotic acids?
What distinguishes a monoprotic acid from diprotic and triprotic acids?
Which of the following correctly describes the differences between monoprotic, diprotic, and triprotic acids?
Which of the following correctly describes the differences between monoprotic, diprotic, and triprotic acids?
Why can't diprotic and triprotic acids be considered monoprotic?
Why can't diprotic and triprotic acids be considered monoprotic?
Which of the following represents an incorrect definition related to acid types?
Which of the following represents an incorrect definition related to acid types?
What is the significance of protons (H+ ions) in the context of acids?
What is the significance of protons (H+ ions) in the context of acids?
What defines an Arrhenius acid?
What defines an Arrhenius acid?
What defines a Brønsted–Lowry base?
What defines a Brønsted–Lowry base?
Which statement describes both Arrhenius and Brønsted–Lowry definitions of acids?
Which statement describes both Arrhenius and Brønsted–Lowry definitions of acids?
Which of the following is NOT a characteristic of an Arrhenius base?
Which of the following is NOT a characteristic of an Arrhenius base?
What is required for a substance to act as a Bronsted–Lowry acid?
What is required for a substance to act as a Bronsted–Lowry acid?
What describes the fundamental difference between Arrhenius and Brønsted–Lowry definitions of bases?
What describes the fundamental difference between Arrhenius and Brønsted–Lowry definitions of bases?
Which option correctly describes the role of a hydrogen ion in acid-base reactions?
Which option correctly describes the role of a hydrogen ion in acid-base reactions?
How do the definitions of acid and base differ under Arrhenius and Brønsted–Lowry theories?
How do the definitions of acid and base differ under Arrhenius and Brønsted–Lowry theories?
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Study Notes
Arrhenius Acid–Base Theory
- An Arrhenius acid releases H+ ions in solution (e.g., HNO3 → H+ + NO3–).
- An Arrhenius base releases OH– ions in solution (e.g., NaOH → Na+ + OH–).
- Ionization refers to forming ions from a molecular compound in solution.
- Dissociation refers to the release of ions from an ionic compound in solution.
Brønsted–Lowry Theory
- Brønsted–Lowry acid: a substance that donates a proton (H+).
- Brønsted–Lowry base: a substance that accepts a proton (H+).
- Conjugate acid-base pairs arise when an acid donates a proton and the base accepts it (e.g., HF and F–).
- Amphiprotic substances can act as both an acid and a base (e.g., H2O).
Mono-, Di-, and Triprotic Acids
- Monoprotic acid: supplies one proton (H+) per molecule (e.g., HCl).
- Diprotic acid: supplies two protons (e.g., H2SO4).
- Triprotic acid: supplies three protons (e.g., H3PO4).
- Polyprotic acids include both diprotic and triprotic acids.
Acid Strength and pKa
- pKa expresses acid strength, defined as pKa = –log Ka.
- A lower pKa value indicates a stronger acid.
- For Ka = 6.3 x 10–4, pKa is approximately 3.20, indicating the solution is acidic.
Buffers
- Buffers resist pH changes upon the addition of small amounts of acid or base.
- A typical buffer system consists of a weak acid and its conjugate base.
- Buffers operate by reacting with added acids or bases:
- When OH– is added, it reacts with H3O+, shifting equilibrium to produce more H3O+.
- When H3O+ is added, the system neutralizes excess H3O+, maintaining pH stability.
Electrolytes and Titrations
- Electrolytes are substances that dissociate into ions in solution, conducting electricity.
- Acid-base titrations involve the gradual addition of an acid or base to determine the concentration of a solution.
- Understanding equivalents and milliequivalents is crucial for measurements in titrations.
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