Podcast
Questions and Answers
What characterizes a Brønsted-Lowry base?
What characterizes a Brønsted-Lowry base?
- It accepts protons. (correct)
- It forms hydronium ions.
- It donates protons.
- It acts as a reagent in oxidation reactions.
Which of the following is an example of an amphoteric substance?
Which of the following is an example of an amphoteric substance?
- HCl
- H2O (correct)
- NaOH
- NH3
What is formed when acetic acid (CH3COOH) donates a proton?
What is formed when acetic acid (CH3COOH) donates a proton?
- Salt (NaCl)
- Conjugate base (CH3COO-) (correct)
- Hydronium ion (H3O+)
- Water (H2O)
According to Bronsted-Lowry theory, a weak acid is characterized by what?
According to Bronsted-Lowry theory, a weak acid is characterized by what?
What is produced in a neutralization reaction?
What is produced in a neutralization reaction?
Which statement about conjugate acid-base pairs is true?
Which statement about conjugate acid-base pairs is true?
What does the Arrhenius theory limit its definition of acids to?
What does the Arrhenius theory limit its definition of acids to?
In the reaction HC2O4- + H+ → H2C2O4, what is the role of HC2O4-?
In the reaction HC2O4- + H+ → H2C2O4, what is the role of HC2O4-?
What characterizes a monobasic acid?
What characterizes a monobasic acid?
Which of the following acids is classified as a weak acid?
Which of the following acids is classified as a weak acid?
What is the characteristic of a strong base according to the Arrhenius definition?
What is the characteristic of a strong base according to the Arrhenius definition?
Which of the following describes a dibasic acid?
Which of the following describes a dibasic acid?
Which is a limitation of the Arrhenius theory of acids and bases?
Which is a limitation of the Arrhenius theory of acids and bases?
What happens to H+ ions in aqueous solutions?
What happens to H+ ions in aqueous solutions?
Which of the following bases is classified as a weak base?
Which of the following bases is classified as a weak base?
According to Bronsted-Lowry theory, what defines a Bronsted-Lowry acid?
According to Bronsted-Lowry theory, what defines a Bronsted-Lowry acid?
What is formed when an acid reacts with a base?
What is formed when an acid reacts with a base?
Which of the following is a strong acid behavior according to the Arrhenius theory?
Which of the following is a strong acid behavior according to the Arrhenius theory?
In neutralization reactions, how is excess hydrochloric acid managed in medicine?
In neutralization reactions, how is excess hydrochloric acid managed in medicine?
Which chemical reaction neutralizes soil acidity in agriculture?
Which chemical reaction neutralizes soil acidity in agriculture?
Which of the following substances acts as a base in the dissociation of nitrous acid in water?
Which of the following substances acts as a base in the dissociation of nitrous acid in water?
What is the product of the reaction between sulfuric acid and limestone?
What is the product of the reaction between sulfuric acid and limestone?
Which of the following is a characteristic of weak acids according to the Brønsted-Lowry theory?
Which of the following is a characteristic of weak acids according to the Brønsted-Lowry theory?
Which neutralization product releases carbon dioxide gas in the reaction with hydrochloric acid?
Which neutralization product releases carbon dioxide gas in the reaction with hydrochloric acid?
Flashcards
Arrhenius Acid
Arrhenius Acid
A substance that releases H+ ions when dissolved in water.
Strong Acid
Strong Acid
An acid that almost completely dissociates into H+ ions in water.
Weak Acid
Weak Acid
An acid that only slightly dissociates into H+ ions in water.
Arrhenius Base
Arrhenius Base
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Strong Base
Strong Base
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Weak Base
Weak Base
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Monobasic Acid
Monobasic Acid
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Brønsted-Lowry Acid
Brønsted-Lowry Acid
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Brønsted-Lowry base
Brønsted-Lowry base
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Conjugate acid
Conjugate acid
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Conjugate base
Conjugate base
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Conjugate acid-base pair
Conjugate acid-base pair
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Neutralization
Neutralization
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Amphoteric substance
Amphoteric substance
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Neutralization Reaction
Neutralization Reaction
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Salt
Salt
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Acid-Base Neutralization
Acid-Base Neutralization
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Dissociation
Dissociation
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Brønsted-Lowry Theory
Brønsted-Lowry Theory
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Study Notes
Arrhenius Theory of Acids and Bases
- Acid: A substance that dissociates in water to produce H+ ions.
- Examples: HCl → H+ + Cl-, H₂SO₄ → 2H+ + SO₄²⁻, H₃PO₄ → 3H+ + PO₄³⁻
- Monobasic acid: Dissociates to give one H+ ion
- Dibasic acid: Dissociates to give two H+ ions
- Tribasic acid: Dissociates to give three H+ ions
- Strong acid: Almost completely dissociates in water to give hydrogen ions. Examples include hydrochloric, sulfuric, and nitric acid.
- Weak acid: Only slightly dissociates in water to give hydrogen ions. Examples include ethanoic and methanoic acid.
- Base: A substance that dissociates in water to produce OH⁻ ions.
- Examples: NaOH → Na⁺ + OH⁻, Mg(OH)₂ → Mg²⁺ + 2OH⁻, Ca(OH)₂ → Ca²⁺ + 2OH⁻
- Strong base: Almost completely dissociates in water to give hydroxide ions. Example Sodium Hydroxide
- Weak base: Slightly dissociates in water to give hydroxide ions. Examples include calcium hydroxide and magnesium hydroxide.
Brønsted-Lowry Theory of Acids and Bases
- Acid: A proton (H⁺) donor
- Base: A proton (H⁺) acceptor
- Conjugate acid-base pair: A pair of acid and base that differ by one proton
- Examples: HCl + H₂O → H₃O⁺ + Cl⁻ (HCl donates a proton, H₂O accepts a proton). NH₃ + H₂O → NH₄⁺ + OH⁻ (NH₃ accepts a proton, H₂O donates a proton).
- Amphoteric substance: A substance that can act as both an acid and a base depending on the reaction. H₂O is an amphoteric substance
Differences Between Arrhenius and Brønsted-Lowry Theories
- Arrhenius Theory: Limited to reactions in water, limited to bases that produce OH⁻ ions, does not take the existence of hydronium ions into account, cannot explain substances that act as both an acid and a base.
- Brønsted-Lowry Theory: Not limited to reactions in water, not limited to bases that produce OH⁻ ions, takes the existence of hydronium ions into account, can explain substances that act as both an acid and a base.
Conjugate Acid-Base Pairs
- Conjugate base: An acid that has lost a proton
- Conjugate acid: A base that has gained a proton
Neutralization
- Definition: The reaction between an acid and a base to form a salt and water.
- Example: HCl + NaOH → NaCl + H₂O
Uses of Neutralization
- Medicine: Neutralizing excess stomach acid.
- Agriculture: Neutralizing soil acidity.
- Environmental Protection: Neutralizing acid rain.
- Miscellaneous: Neutralizing acids or bases in food, toothpaste, and shampoo, neutralizing stings of wasps.
Exam Questions (Examples)
- Strong vs Weak Acids/Bases: Strong acids/bases dissociate almost completely in water, while weak acids/bases only slightly dissociate.
- Conjugate Bases: These are formed when an acid loses a proton. Stronger acids tend to have weaker conjugate bases.
- Acid-Base Reactions: Consider the balanced equations for these reactions.
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Description
Test your understanding of the Arrhenius theory, which defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. This quiz covers the properties of strong and weak acids and bases, their dissociation in water, and examples of each. Perfect for students studying chemistry.
