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Questions and Answers
List the classes of electrolytes.
List the classes of electrolytes.
Acids, bases, and salts.
Explain the difference between acids, bases, and salts.
Explain the difference between acids, bases, and salts.
Acids contain hydronium ions, bases contain hydroxide ions, and salts are ionic compounds made from cations and anions.
List the properties of aqueous acids.
List the properties of aqueous acids.
- Taste sour, 2. pH less than 7.0, 3. Corrosive, 4. Neutralize bases, 5. Change the colors of indicators, 6. React with metals, 7. React with carbonates to produce CO2, 8. Conduct electric current.
List the properties of aqueous bases.
List the properties of aqueous bases.
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Explain the difference between a) a strong acid and a weak acid, and b) a strong base and a weak base.
Explain the difference between a) a strong acid and a weak acid, and b) a strong base and a weak base.
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Explain the difference between a binary acid and an oxyacid.
Explain the difference between a binary acid and an oxyacid.
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Define acid and base according to the Arrhenius concept.
Define acid and base according to the Arrhenius concept.
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Define acid and base according to the Bronsted-Lowry concept.
Define acid and base according to the Bronsted-Lowry concept.
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Distinguish between a monoprotic, a diprotic, and a triprotic acid. Give an example of each.
Distinguish between a monoprotic, a diprotic, and a triprotic acid. Give an example of each.
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What is a conjugate acid?
What is a conjugate acid?
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What is a conjugate base?
What is a conjugate base?
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What is an amphoteric substance? Give 2 examples.
What is an amphoteric substance? Give 2 examples.
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Define acid and base according to the Lewis concept.
Define acid and base according to the Lewis concept.
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Which of the three acid definitions is the broadest? Explain.
Which of the three acid definitions is the broadest? Explain.
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Define pH.
Define pH.
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What is the pH scale?
What is the pH scale?
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What is the relationship between the concentration of the hydronium ion and the concentration of the hydroxide ion when the pH is 7 (neutral)? When the pH is less than 7? When the pH is greater than 7?
What is the relationship between the concentration of the hydronium ion and the concentration of the hydroxide ion when the pH is 7 (neutral)? When the pH is less than 7? When the pH is greater than 7?
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What is an indicator?
What is an indicator?
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Identify the color of the indicator in an acid and in a base: litmus.
Identify the color of the indicator in an acid and in a base: litmus.
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Identify the color of the indicator in an acid and in a base: phenolphthalein.
Identify the color of the indicator in an acid and in a base: phenolphthalein.
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What is a neutralization reaction?
What is a neutralization reaction?
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Study Notes
Acids, Bases, and Salts
- Classes of electrolytes include acids, bases, and salts.
Differences Among Acids, Bases, and Salts
- Acids: Contain hydronium ions (H3O+).
- Bases: Contain hydroxide ions (OH-).
- Salts: Ionic compounds composed of cations and anions.
Properties of Aqueous Acids
- Have a sour taste.
- pH is less than 7.0.
- Are corrosive.
- Neutralize bases during reactions.
- Change the color of indicators.
- React with metals, producing hydrogen gas.
- React with carbonates to yield carbon dioxide (CO2).
- Conduct electric current.
Properties of Aqueous Bases
- Have a bitter taste.
- pH is greater than 7.0.
- Are caustic.
- Neutralize acids during reactions.
- Change the color of indicators.
- Can dissolve fats and oils.
- Feel slippery to the touch.
- Conduct electric current.
Strong vs. Weak Electrolytes
- Strong electrolytes: Completely ionize in water, such as strong acids and bases.
- Weak electrolytes: Only partially ionize in water.
Binary Acids vs. Oxyacids
- Binary acids: Consist of only two elements.
- Oxyacids: Contain two elements plus oxygen, often involving polyatomic ions.
Arrhenius Concept of Acids and Bases
- Acid: Donates hydrogen ions (H+).
- Base: Donates hydroxide ions (OH-).
Bronsted-Lowry Concept of Acids and Bases
- Acid: Proton donor.
- Base: Proton acceptor.
Types of Acids
- Monoprotic: Donate one hydrogen ion (e.g., HF).
- Diprotic: Donate two hydrogen ions (e.g., H2SO4).
- Triprotic: Donate three hydrogen ions (e.g., H3PO4).
Conjugate Acids and Bases
- Conjugate acid: Formed when a base accepts a proton.
- Conjugate base: Formed when an acid donates a proton.
Amphoteric Substances
- Can act as both an acid and a base; examples include water (H2O) and ammonia (NH3).
Lewis Concept of Acids and Bases
- Acid: Electron pair acceptor.
- Base: Electron pair donor.
- This definition is broader and includes substances without hydrogen.
pH Definition
- Describes the acidity of a solution.
pH Scale
- Based on the logarithm of hydronium ion concentration, ranging from 0 to 14.
Relationship of Ion Concentrations and pH
- At pH 7: Hydronium concentration equals hydroxide concentration (neutral).
- pH less than 7: Greater hydronium concentration.
- pH greater than 7: Greater hydroxide concentration.
Indicators
- Sensitive dyes that change color with pH changes.
Indicator Colors
- Litmus: Red in an acid, blue in a base.
- Phenolphthalein: Colorless in an acid, bright pink in a base.
Neutralization Reactions
- Result from the reaction between an acid and a base, producing water (H2O) and salt.
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Description
Test your knowledge on acids, bases, and salts with these flashcards. Each card covers essential definitions and differences between these important classes of electrolytes. Perfect for students studying chemistry concepts related to solutions and ionic compounds.
