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pH Revisited definitions

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  • pH
    A logarithmic measure reflecting the effective concentration of hydrogen ions in a solution, influenced by temperature and ionic environment.
  • Kw
    The equilibrium constant for water ionization, varying with temperature and affecting neutral solution calculations.
  • Ionic Strength
    A quantitative measure of the total concentration and charge of ions in solution, impacting activity coefficients and solubility.
  • Activity Coefficient
    A correction factor adjusting ion concentrations to account for non-ideal solution behavior due to ionic interactions.
  • Neutral Solution
    A state where hydrogen ion and hydroxide ion concentrations are equal, typically in pure water.
  • Non-Common Ion Effect
    The influence of ions not shared with the solute, altering ionic strength and thus affecting solubility and pH.
  • Ksp
    The solubility product constant, representing the equilibrium between a solid ionic compound and its dissolved ions.
  • Hydroxide Ion
    A negatively charged ion, its concentration is crucial for determining pOH and, subsequently, pH.
  • Saturated Solution
    A solution containing the maximum amount of dissolved solute, with excess present as undissolved solid.
  • Temperature Dependence
    The property of equilibrium constants, such as Kw, to change with temperature, affecting calculations like pH.
  • Solubility
    The extent to which a substance dissolves in a solvent, influenced by ionic strength and activity coefficients.
  • Hydrogen Ion
    A positively charged ion, its effective concentration determines the acidity and pH of a solution.
  • pOH
    A logarithmic measure of hydroxide ion activity, used to calculate pH in basic solutions.
  • Ionic Compound
    A substance composed of cations and anions, whose dissolution and interactions affect solution properties like pH.
  • Equilibrium Constant
    A value expressing the ratio of product and reactant activities at equilibrium, central to calculations involving pH and solubility.