Skip to main content
뒤로

Buffer Solution definitions

컨트롤 버튼이 '내비게이션' 모드로 변경되었습니다.
1/15
  • Buffer
    Substance that maintains stable pH when small amounts of strong acids or bases are added, crucial for biochemical processes.
  • pH
    Measure of hydrogen ion concentration, indicating acidity or basicity; stability is essential for enzyme activity.
  • Henderson-Hasselbalch Equation
    Mathematical expression relating pH, pKa, and ratio of conjugate base to acid, used to prepare buffer solutions.
  • pKa
    Value representing the acid dissociation constant; central to determining effective buffering range of weak acids.
  • Conjugate Base
    Species formed when a weak acid loses a proton; pairs with its acid to create an effective buffer system.
  • Conjugate Acid
    Species formed when a base gains a proton; partners with its base in buffer systems to resist pH changes.
  • Acetic Acid
    Monoprotic weak acid with formula CH3COOH; effective buffer within pH range 3.8 to 5.8 due to its pKa of 4.8.
  • Titration Curve
    Graph showing pH changes as titrant is added; inflection point indicates pKa and effective buffering range.
  • Phosphate Buffer System
    Intracellular buffer using dihydrogen phosphate and hydrogen phosphate; effective near pKa of 7.2.
  • Bicarbonate Buffer System
    Extracellular buffer composed of carbonic acid and bicarbonate; maintains blood pH near 7.4.
  • Dihydrogen Phosphate
    Component of phosphate buffer system; helps maintain intracellular pH within effective buffering range.
  • Hydrogen Phosphate
    Partner in phosphate buffer system; works with dihydrogen phosphate to stabilize cell pH.
  • Carbonic Acid
    Weak acid in bicarbonate buffer system; pKa of 6.4, crucial for maintaining extracellular pH.
  • Bicarbonate
    Conjugate base in bicarbonate buffer system; interacts with carbonic acid to regulate blood pH.
  • Homeostasis
    Biological state where internal conditions, such as pH, are maintained for optimal enzyme and cellular function.