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Dependence of Solubility on pH definitions

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  • Activity Coefficient
    A factor that corrects for non-ideal behavior of ions in solution, influenced by ionic strength and ion charge.
  • Ionic Strength
    A measure of the total concentration of ions in solution, weighted by the square of each ion's charge.
  • Extended Debye-Hückel Equation
    A formula relating activity coefficient to ionic strength, ion charge, and ion size parameter for accurate predictions.
  • Size Parameter
    A value, often in nanometers, representing the effective diameter of an ion in solution.
  • Davies Equation
    An empirical formula for estimating activity coefficients, especially for monovalent ions when ion size is unknown.
  • Cation
    A positively charged ion, which can be acidic, neutral, or basic depending on its charge and group.
  • Anion
    A negatively charged ion, classified as basic or neutral based on the acid formed when combined with H+.
  • Acidic Salt
    A compound that increases solution acidity due to the presence of an acidic cation.
  • Basic Anion
    A negatively charged ion that forms a weak acid upon reaction with H+, increasing solubility in acidic conditions.
  • Neutral Anion
    A negatively charged ion that forms a strong acid with H+, resulting in negligible basicity.
  • Amphoteric Species
    An ion or molecule capable of acting as either an acid or a base, with solubility affected by pH.
  • Le Chatelier's Principle
    A rule stating that a system at equilibrium will adjust to counteract changes, affecting solubility with pH shifts.
  • Transition Metal
    A metal ion, typically requiring a charge of +2 or higher to exhibit acidic behavior in solution.
  • Main Group Metal
    A metal ion from groups 1A to 3A, needing a charge of +3 or higher to be considered acidic.
  • Monovalent Ion
    An ion with a single positive or negative charge, such as sodium or chloride, often used with the Davies equation.