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Questions and Answers
What is the definition of an acid according to the Arrhenius Theory?
What is the definition of an acid according to the Arrhenius Theory?
What is the pH of a neutral solution?
What is the pH of a neutral solution?
Which of the following is an example of a strong acid?
Which of the following is an example of a strong acid?
What is the purpose of an acid-base indicator?
What is the purpose of an acid-base indicator?
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According to the Bronsted-Lowry Theory, what is a conjugate acid?
According to the Bronsted-Lowry Theory, what is a conjugate acid?
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What is the formula for pH?
What is the formula for pH?
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What type of reaction occurs between an acid and a base to form a salt and water?
What type of reaction occurs between an acid and a base to form a salt and water?
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Which of the following is an example of a weak base?
Which of the following is an example of a weak base?
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Study Notes
Arrhenius Theory
- Acids: substances that donate a proton (H+)
- Bases: substances that accept a proton (OH-)
Bronsted-Lowry Theory
- Acids: substances that donate a proton (H+)
- Bases: substances that accept a proton
- Conjugate acid: the species formed when a base accepts a proton
- Conjugate base: the species formed when an acid donates a proton
pH Scale
- Measures the concentration of hydrogen ions (H+) in a solution
- pH = -log[H+]
- pH 7: neutral (neither acidic nor basic)
- pH < 7: acidic
- pH > 7: basic
Strong and Weak Acids and Bases
- Strong acids: completely dissociate in water, releasing all H+ ions
- Examples: HCl, HNO3, H2SO4
- Weak acids: partially dissociate in water, releasing some H+ ions
- Examples: CH3COOH, HCN, HF
- Strong bases: completely dissociate in water, releasing all OH- ions
- Examples: NaOH, KOH, Ca(OH)2
- Weak bases: partially dissociate in water, releasing some OH- ions
- Examples: NH3, CO3^2-, PO4^3-
Acid-Base Reactions
- Neutralization: reaction between an acid and a base to form a salt and water
- Example: HCl + NaOH → NaCl + H2O
- Acid-base equilibrium: balance between the forward and reverse reactions
- Example: HCl + H2O ⇌ H3O+ + Cl-
Acid-Base Indicators
- Substances that change color in response to changes in pH
- Used to determine the pH of a solution
- Examples: litmus, phenolphthalein, methyl orange
Arrhenius Theory
- Acids are defined as substances that donate a proton (H+)
- Bases are defined as substances that accept a proton (OH-)
Bronsted-Lowry Theory
- Acids are defined as substances that donate a proton (H+)
- Bases are defined as substances that accept a proton
- Conjugate acid is the species formed when a base accepts a proton
- Conjugate base is the species formed when an acid donates a proton
pH Scale
- Measures the concentration of hydrogen ions (H+) in a solution
- Calculated using the formula: pH = -log[H+]
- pH 7 is neutral, meaning neither acidic nor basic
- Solutions with pH < 7 are acidic
- Solutions with pH > 7 are basic
Strong and Weak Acids and Bases
- Strong acids completely dissociate in water, releasing all H+ ions
- Examples: HCl, HNO3, H2SO4
- Weak acids partially dissociate in water, releasing some H+ ions
- Examples: CH3COOH, HCN, HF
- Strong bases completely dissociate in water, releasing all OH- ions
- Examples: NaOH, KOH, Ca(OH)2
- Weak bases partially dissociate in water, releasing some OH- ions
- Examples: NH3, CO3^2-, PO4^3-
Acid-Base Reactions
- Neutralization reactions occur between an acid and a base to form a salt and water
- Example: HCl + NaOH → NaCl + H2O
- Acid-base equilibrium is the balance between the forward and reverse reactions
- Example: HCl + H2O ⇌ H3O+ + Cl-
Acid-Base Indicators
- Are substances that change color in response to changes in pH
- Used to determine the pH of a solution
- Examples: litmus, phenolphthalein, methyl orange
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Description
Understand the concepts of acids and bases according to Arrhenius and Bronsted-Lowry theories, and learn about the pH scale which measures the concentration of hydrogen ions in a solution.
