Questions and Answers
Which of the following are properties of acids? (Select all that apply)
Which of the following are properties of bases? (Select all that apply)
List 7 strong acids.
Hydrochloric acid, Hydrobromic acid, Hydroiodic acid, Nitric acid, Sulfuric acid, Chloric acid, Perchloric acid
How does an acid become a conjugate base?
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How does a base become a conjugate acid?
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What is the conjugate base of H2CO3?
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What is the conjugate base of H2S?
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What is the conjugate base of HF?
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What is the conjugate base of HSO4-?
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What is the conjugate base of HCO3-?
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What is the conjugate acid of CO32-?
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What is the conjugate acid of HCO3-?
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What is the conjugate acid of H2O?
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Double-headed arrows mean ________.
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What is it called when water reacts with itself?
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The majority of weak acids are in the form of what?
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All aqueous solutions contain both H3O+ and OH-.
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What is the ion-product constant for water?
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What does pH express?
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Buffered solutions contain what?
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Study Notes
Properties of Acids
- Have a sour taste and are corrosive.
- Change color of vegetable dyes.
- React with "active" metals and carbonates to produce CO2.
- React with bases to form ionic salts.
Properties of Bases
- Also referred to as alkali, with a bitter taste and slippery feel.
- Change color of vegetable dyes.
- React with acids to form ionic salts, a process called neutralization.
Strong Acids
- Notable strong acids include hydrochloric acid, hydrobromic acid, hydroiodic acid, nitric acid, sulfuric acid, chloric acid, and perchloric acid.
Conjugate Bases
- An acid becomes a conjugate base by losing 1 H+ ion.
- Common conjugate bases include:
- H2CO3 transforms to HCO3-
- H2S transforms to HS-
- HF transforms to F-
- HSO4- transforms to SO42-
- HCO3- transforms to CO32-
Conjugate Acids
- A base becomes a conjugate acid by gaining 1 H+ ion.
- Example transformations include:
- CO32- converts to HCO3-
- HCO3- converts to H2CO3
- H2O converts to H3O+
Acid-Base Equilibria
- Double-headed arrows signify weak acids or bases, indicating partial dissociation.
- Autoionization occurs when water reacts with itself, producing H3O+ and OH- ions.
Characteristics of Weak Acids
- The majority of weak acids exist primarily in the form of reactants in solution.
Aqueous Solutions
- All aqueous solutions contain both H3O+ and OH- ions.
Ion-Product Constant for Water
- Represented by Kw, which defines the equilibrium constant for water's autoionization.
pH Concept
- pH quantifies the hydrogen ion concentration, expressed as the negative logarithm of [H+].
Buffered Solutions
- Consist of a weak acid and the salt of its conjugate base, or a weak base and the salt of its conjugate acid, used to resist changes in pH.
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Test your knowledge on the properties of acids and bases with these informative flashcards. Learn key definitions and characteristics that differentiate these two important concepts in chemistry. Perfect for students looking to reinforce their understanding of acid-base chemistry.
