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Ionic Strength of Soluble Salts definitions

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  • Ionic Solid
    A compound composed of ions held together by electrostatic forces, exhibiting low solubility in water.
  • Equilibrium
    A state where the rate of dissolution and precipitation of ions in solution are equal, resulting in constant concentrations.
  • Ksp
    A constant representing the product of ion concentrations at equilibrium for a sparingly soluble salt.
  • Solubility
    The maximum amount of an ionic compound that can dissolve in a solvent to form a saturated solution.
  • Common Ion Effect
    A phenomenon where the presence of a shared ion reduces the solubility of an ionic compound by shifting equilibrium.
  • Le Chatelier's Principle
    A rule predicting how a system at equilibrium responds to disturbances, favoring the direction that counteracts the change.
  • Crystallization
    The process where dissolved ions recombine to form a solid, often favored by the common ion effect.
  • Aqueous Solution
    A homogeneous mixture where water acts as the solvent for dissolved ions or molecules.
  • Ionic Strength
    A measure quantifying the total concentration and charge of all ions present in a solution, affecting solubility.
  • Charge Squared
    A mathematical factor in the ionic strength equation, emphasizing the influence of ion charge on solution properties.
  • Saturated Solution
    A solution containing the maximum concentration of dissolved ions, in dynamic equilibrium with undissolved solid.
  • Precipitation
    The formation of a solid from ions in solution when their product exceeds the solubility product constant.
  • Non Common Ion
    An ion present in solution that does not participate in the equilibrium of the ionic solid, influencing solubility via ionic strength.
  • Solubility Product Constant
    A specific equilibrium constant for the dissolution of a sparingly soluble ionic compound in water.
  • Dissociation
    The separation of an ionic solid into its constituent ions when introduced into a solvent.