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Buffers definitions

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  • Buffer
    A solution that resists drastic pH changes by neutralizing added acids or bases using a weak acid and its conjugate base or vice versa.
  • Weak Acid
    A substance that partially dissociates in water, providing limited H+ ions, and forms the acidic component of a buffer.
  • Conjugate Base
    A species formed when a weak acid loses an H+ ion, often paired with a metal in buffer solutions for stability.
  • pH
    A measure of hydrogen ion concentration, indicating the acidity or basicity of a solution, which buffers help stabilize.
  • Buffer Capacity
    The effectiveness of a buffer, which increases with higher concentrations of weak acid and conjugate base.
  • Buffer Range
    The ratio window (10:1 to 1:10) of weak acid to conjugate base concentrations where a buffer works most effectively.
  • Strong Acid
    A substance that completely dissociates in water, providing a high concentration of H+ ions, which can destroy buffers if added in excess.
  • Strong Base
    A substance that fully dissociates in water, yielding a high concentration of OH- ions, capable of overwhelming a buffer.
  • Half Equivalence Point
    The stage in a titration where equal amounts of weak acid and conjugate base exist, resulting in an ideal buffer.
  • Neutralization
    The process where an acid and a base react to minimize pH changes, central to how buffers function.
  • Molarity
    A unit expressing concentration as moles of solute per liter of solution, crucial for buffer calculations.
  • Titration
    A laboratory technique involving gradual addition of one solution to another to study reactions, often used to analyze buffer behavior.
  • Acid-Base Pair
    A combination of a weak acid and its conjugate base or a weak base and its conjugate acid, forming the foundation of buffer systems.
  • Dilution
    The process of adding water to a solution, which does not affect buffer effectiveness due to proportional concentration changes.