Acids and Bases Characteristics

Acids

• Definition: A substance that donates a proton (H+ ion) in a solution
• Characteristics:
  • Sour taste
  • Conduct electricity
  • Turn litmus paper red
  • React with metals to produce hydrogen gas
• Examples:
  • Hydrochloric acid (HCl)
  • Sulfuric acid (H2SO4)
  • Nitric acid (HNO3)
  • Acetic acid (CH3COOH)

Bases

• Definition: A substance that accepts a proton (H+ ion) in a solution
• Characteristics:
  • Bitter taste
  • Feel slippery to the touch
  • Conduct electricity
  • Turn litmus paper blue
  • React with oils to produce soap
• Examples:
  • Sodium hydroxide (NaOH)
  • Calcium hydroxide (Ca(OH)2)
  • Ammonia (NH3)

pH Scale

• Measures the concentration of hydrogen ions (H+) in a solution
• pH = -log[H+]
• Range: 0-14
• Acidic: pH < 7
• Neutral: pH = 7
• Basic: pH > 7

Salt

• Definition: A substance formed by the reaction of an acid and a base
• Characteristics:
  • Neutral in taste
  • Neither acidic nor basic
  • Formed by the reaction of an acid and a base
• Examples:
  • Sodium chloride (NaCl) - formed by the reaction of HCl and NaOH
  • Calcium carbonate (CaCO3) - formed by the reaction of H2CO3 and Ca(OH)2

Strong and Weak Acids and Bases

• Strong acids:
  • Completely dissociate in water
  • Examples: HCl, H2SO4, HNO3
• Weak acids:
  • Partially dissociate in water
  • Examples: CH3COOH, H2CO3
• Strong bases:
  • Completely dissociate in water
  • Examples: NaOH, Ca(OH)2
• Weak bases:
  • Partially dissociate in water
  • Examples: NH3, trimethylamine (N(CH3)3)

Importance of Acid-Base Chemistry

• Biological systems: pH affects enzyme activity, protein structure, and cell function
• Environmental systems: pH affects soil chemistry, water quality, and ecosystem health
• Industrial applications: pH control is crucial in manufacturing processes, such as food processing and pharmaceutical production

Acids

• Donate a proton (H+ ion) in a solution
• Typically have a sour taste
• Conduct electricity and turn litmus paper red
• React with metals to produce hydrogen gas
• Examples include hydrochloric acid (HCl), sulfuric acid (H2SO4), nitric acid (HNO3), and acetic acid (CH3COOH)

Bases

• Accept a proton (H+ ion) in a solution
• Typically have a bitter taste and feel slippery to the touch
• Conduct electricity and turn litmus paper blue
• React with oils to produce soap
• Examples include sodium hydroxide (NaOH), calcium hydroxide (Ca(OH)2), and ammonia (NH3)

pH Scale

• Measures the concentration of hydrogen ions (H+) in a solution
• pH is calculated using the formula pH = -log[H+]
• Ranges from 0 to 14, with 7 being neutral
• Acidic solutions have a pH below 7, while basic solutions have a pH above 7

Salts

• Formed by the reaction of an acid and a base
• Neutral in taste and neither acidic nor basic
• Examples include sodium chloride (NaCl) and calcium carbonate (CaCO3)

Strong and Weak Acids and Bases

• Strong acids completely dissociate in water, releasing all H+ ions
• Examples of strong acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3)
• Weak acids partially dissociate in water, releasing some H+ ions
• Examples of weak acids include acetic acid (CH3COOH) and carbonic acid (H2CO3)
• Strong bases completely dissociate in water, releasing all OH- ions
• Examples of strong bases include sodium hydroxide (NaOH) and calcium hydroxide (Ca(OH)2)
• Weak bases partially dissociate in water, releasing some OH- ions
• Examples of weak bases include ammonia (NH3) and trimethylamine (N(CH3)3)

Importance of Acid-Base Chemistry

• pH affects enzyme activity, protein structure, and cell function in biological systems
• pH affects soil chemistry, water quality, and ecosystem health in environmental systems
• pH control is crucial in industrial applications, such as food processing and pharmaceutical production