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Strong Acid-Strong Base Titrations definitions

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  • Titration
    Analytical process where a solution of known concentration is gradually added to another to determine its concentration.
  • Strong Acid
    Substance that dissociates completely in water, producing a high concentration of hydrogen ions.
  • Strong Base
    Compound that fully dissociates in solution, yielding a high concentration of hydroxide ions.
  • ICF Chart
    Tabular method using moles to track initial, change, and final amounts during reactions with complete dissociation.
  • Equivalence Point
    Stage in titration where moles of acid and base are equal, resulting in complete neutralization.
  • Analyte
    Substance in a titration whose concentration is being determined by reaction with a titrant.
  • Titrant
    Solution of known concentration added to react with the analyte during titration.
  • Molarity
    Measure of concentration expressed as moles of solute per liter of solution.
  • pH
    Logarithmic scale representing the hydrogen ion concentration, indicating acidity or basicity.
  • pOH
    Logarithmic measure of hydroxide ion concentration, related to pH by their sum equaling 14 at 25°C.
  • Conjugate Base
    Species formed when an acid donates a proton during a neutralization reaction.
  • Neutral Salt
    Product of strong acid-strong base titration that does not affect pH if activity coefficients are ignored.
  • Limiting Reactant
    Reactant present in the smallest mole amount, determining the extent of reaction completion.
  • Conservation of Mass
    Principle stating matter is neither created nor destroyed, only transformed during chemical reactions.
  • Activity Coefficient
    Factor accounting for deviations from ideal behavior in ion interactions, often ignored in basic titration calculations.