Acid-Base Chemistry Quiz

Acid-Base Chemistry

Definition

• Acid: a substance that donates a proton (H+)
• Base: a substance that accepts a proton (H+)

pH Scale

• pH: a measure of acidity/basicity, ranging from 0-14
• pH 7: neutral (neither acidic nor basic)
• pH < 7: acidic
• pH > 7: basic

pH Calculation

• pH = -log[H+]
• [H+] = concentration of hydrogen ions (in moles per liter)

Strong and Weak Acids/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, HCO3-
• Strong bases: completely dissociate in water, releasing all OH- ions
  • Examples: NaOH, KOH
• Weak bases: partially dissociate in water, releasing some OH- ions
  • Examples: NH3, CH3NH2

Acid-Base Reactions

• Neutralization reaction: acid + base → salt + water
  • Example: HCl + NaOH → NaCl + H2O
• Acid-base conjugate pairs: acid + base ⇌ conjugate acid + conjugate base
  • Example: HCl + H2O ⇌ H3O+ + Cl-

Blood pH Regulation

• Blood pH range: 7.35-7.45
• Regulation mechanisms:
  • Respiratory system: controls CO2 levels, which affect pH
  • Renal system: controls H+ and HCO3- levels
  • Buffers: help maintain pH homeostasis

Acid-Base Chemistry

Definition and pH Scale

• Acid: a substance that donates a proton (H+)
• Base: a substance that accepts a proton (H+)
• pH: a measure of acidity/basicity, ranging from 0-14
• pH 7: neutral (neither acidic nor basic)
• pH < 7: acidic
• pH > 7: basic

pH Calculation

• pH = -log[H+], where [H+] is the concentration of hydrogen ions (in moles per liter)

Strong and Weak Acids/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, HCO3-
• Strong bases:
  • Completely dissociate in water, releasing all OH- ions
  • Examples: NaOH, KOH
• Weak bases:
  • Partially dissociate in water, releasing some OH- ions
  • Examples: NH3, CH3NH2

Acid-Base Reactions

• Neutralization reaction:
  • Acid + base → salt + water
  • Example: HCl + NaOH → NaCl + H2O
• Acid-base conjugate pairs:
  • Acid + base ⇌ conjugate acid + conjugate base
  • Example: HCl + H2O ⇌ H3O+ + Cl-

Blood pH Regulation

• Blood pH range: 7.35-7.45
• Regulation mechanisms:
  • Respiratory system: controls CO2 levels, which affect pH
  • Renal system: controls H+ and HCO3- levels
  • Buffers: help maintain pH homeostasis

Test your knowledge of acid-base chemistry, including the definition of acids and bases, pH scale, pH calculation, and strong and weak acids/bases.