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Titrations: Weak Base-Strong Acid definitions

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  • Titration
    A laboratory method to determine the concentration of a solute in a solution by adding a titrant of known concentration.
  • Weak Base
    A base that does not completely ionize in solution, resulting in a higher pH than a strong base.
  • Strong Acid
    An acid that completely ionizes in solution, significantly lowering the pH.
  • Equivalence Point
    The stage in titration where the moles of acid equal the moles of base, resulting in neutralization.
  • Buffer
    A solution that resists changes in pH when small amounts of acid or base are added.
  • Henderson-Hasselbalch Equation
    An equation used to calculate the pH of a buffer solution using the concentration of acid and its conjugate base.
  • ICF Chart
    A tool used to track the initial, change, and final amounts of reactants and products in a chemical reaction.
  • Molarity
    A measure of the concentration of a solute in a solution, expressed as moles of solute per liter of solution.
  • Conjugate Acid
    The species formed when a base gains a proton, often present in buffer solutions.
  • Neutralization
    A chemical reaction in which an acid and a base react to form water and a salt, resulting in a neutral pH.
  • Ionization
    The process by which an atom or molecule gains or loses electrons to form ions, affecting pH.