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Buffer definitions

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Terms in this set (15)

  • Buffer
    A solution that resists drastic changes in pH, containing a weak acid and its conjugate base or a weak base and its conjugate acid.
  • Weak Acid
    An acid that partially dissociates in solution, such as HF, contributing to buffer formation.
  • Conjugate Base
    The species formed when a weak acid loses a proton, often combined with a metal, like NaF.
  • pH
    A measure of the acidity or basicity of a solution, influenced by the presence of buffers.
  • Buffer Capacity
    The ability of a buffer to neutralize added acids or bases, enhanced by higher concentrations of buffer components.
  • Buffer Range
    The pH range over which a buffer effectively neutralizes added acids or bases, typically between a 10:1 or 1:10 ratio.
  • Ideal Buffer
    A buffer where the concentrations of the weak acid and conjugate base are equal, providing optimal pH stability.
  • Half Equivalence Point
    The point in a titration where the concentration of the weak acid equals that of its conjugate base, forming an ideal buffer.
  • Henderson-Hasselbalch Equation
    An equation used to calculate the pH of a buffer solution, involving pKa and the ratio of conjugate base to weak acid.
  • pKa
    The negative logarithm of the acid dissociation constant, used in the Henderson-Hasselbalch equation to find buffer pH.
  • Strong Acid
    An acid that completely dissociates in solution, potentially destroying a buffer if added in excess.
  • Strong Base
    A base that completely dissociates in solution, potentially destroying a buffer if added in excess.
  • Molarity
    A measure of concentration, used to express the amount of solute in a given volume of solution, relevant in buffer calculations.
  • Titration
    A technique to determine the concentration of a solution, involving the gradual addition of a titrant to a known volume of analyte.
  • Neutralization
    The reaction between an acid and a base to form water and a salt, a key process in buffer function.