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Titrations and Titration Curves definitions

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  • Redox Titration
    Analytical method tracking concentration changes of reacting species as titrant is added, often visualized with a titration curve.
  • Titration Curve
    Graph showing how a measured property, like pCl, changes as titrant is added, highlighting key points such as equivalence.
  • Analyte
    Substance in a solution whose concentration is determined during titration, often present in excess before equivalence.
  • Titrant
    Solution of known concentration added to react with the analyte, used to determine analyte quantity.
  • Equivalence Point
    Stage in titration where stoichiometric amounts of analyte and titrant have reacted, often marked by a sharp change in the curve.
  • Equivalence Volume
    Volume of titrant required to reach the equivalence point, calculated using the molarity and volume relationship.
  • Precipitation Reaction
    Process where ions in solution combine to form an insoluble solid, often used to signal the endpoint in titrations.
  • Solubility Product Constant
    Equilibrium constant (Ksp) for the dissolution of a sparingly soluble ionic compound, used to calculate ion concentrations.
  • Formation Constant
    Inverse of the solubility product constant, indicating the favorability of solid formation from ions in solution.
  • pCl
    Negative logarithm of chloride ion concentration, used to track changes during titration, similar to pH for acids.
  • Indicator
    Substance that changes color at or near the endpoint, helping to visually identify titration completion.
  • Endpoint
    Moment in titration when the indicator signals completion, which may not exactly match the equivalence point.
  • Millimole
    Unit representing one-thousandth of a mole, useful for calculations involving small solution volumes in titrations.
  • Stoichiometry
    Quantitative relationship between reactants and products, essential for calculating amounts at various titration stages.
  • Potentiometric Titration
    Technique using electrical potential measurements to determine titration progress and endpoint, often more precise than visual indicators.