pH Scale and Strong Acids
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Questions and Answers

What is the pH of a solution with a hydrogen ion concentration of 0.01 M?

  • 1
  • 12
  • 2 (correct)
  • 10

    • Which of the following characteristics is common to both strong and weak acids?

  • Partial ionization in water (correct)
  • Production of a high concentration of H+ ions
  • Complete ionization in water
  • High dissociation constant (Ka)

    • What is the pH of a solution with an equimolar concentration of hydrogen ions (H+) and hydroxide ions (OH-)?

  • 0
  • 10
  • 7 (correct)
  • 14

    • Which acid is an example of a weak acid?

    <p>Acetic acid (CH3COOH)</p> Signup and view all the answers

    What is the effect of increasing the concentration of hydrogen ions (H+) in a solution on its pH?

    <p>Decreases the pH</p> Signup and view all the answers

    Study Notes

    pH Scale

    • The pH scale measures the concentration of hydrogen ions (H+) in a solution
    • pH = -log[H+]
    • pH ranges from 0 to 14, with:
      • pH 7: neutral (equimolar concentrations of H+ and OH-)
      • pH < 7: acidic (excess H+)
      • pH > 7: basic (excess OH-)

    Strong Acids

    • Completely dissociate in water to produce H+ and an anion
    • Examples:
      1. Hydrochloric acid (HCl)
      2. Sulfuric acid (H2SO4)
      3. Nitric acid (HNO3)
      4. Perchloric acid (HClO4)
    • Characteristics:
      • High dissociation constant (Ka)
      • Completely ionize in water
      • Produce a high concentration of H+ ions

    Weak Acids

    • Partially dissociate in water to produce H+ and an anion
    • Examples:
      1. Acetic acid (CH3COOH)
      2. Carbonic acid (H2CO3)
      3. Citric acid (C6H8O7)
      4. Formic acid (HCOOH)
    • Characteristics:
      • Low dissociation constant (Ka)
      • Partially ionize in water
      • Produce a low concentration of H+ ions

    pH Scale

    • Measures the concentration of hydrogen ions (H+) in a solution
    • Calculated using the formula pH = -log[H+]
    • Ranges from 0 to 14
    • Neutral pH: 7, where H+ and OH- concentrations are equimolar
    • Acidic pH: < 7, with excess H+ ions
    • Basic pH: > 7, with excess OH- ions

    Strong Acids

    • Completely dissociate in water to produce H+ and an anion
    • Characteristics:
    • High dissociation constant (Ka)
    • Complete ionization in water
    • Produce high concentrations of H+ ions
    • Examples:
    • Hydrochloric acid (HCl)
    • Sulfuric acid (H2SO4)
    • Nitric acid (HNO3)
    • Perchloric acid (HClO4)

    Weak Acids

    • Partially dissociate in water to produce H+ and an anion
    • Characteristics:
    • Low dissociation constant (Ka)
    • Partial ionization in water
    • Produce low concentrations of H+ ions
    • Examples:
    • Acetic acid (CH3COOH)
    • Carbonic acid (H2CO3)
    • Citric acid (C6H8O7)
    • Formic acid (HCOOH)

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    Description

    Learn about the pH scale, its calculation, and characteristics of strong acids. Understand how to identify acidic, basic, and neutral solutions.

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