Table of solubility product constants of substances
Table shows solubility equilibriums of selected substances, mainly sparingly soluble salts and hydroxides.

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Some facts#

  • If the substance MmXxM_mX_x dissociates in the solution according to the reaction:
    MmXx    mMx++xXmM_mX_x \iff m M^{x+} + x X^{m-}
    then its solubility equilibrium is defined as below:
    Ksp=[Mx+]m[Xm]xK_{sp} = \left[\mathrm M^{x+}\right]^m \left[\mathrm X^{m-}\right]^x

    where:
    • KspK_{sp} - solubility quilibrium of substance,
    • [Mx+]m\left[\mathrm M^{x+}\right]^m - molar concentration of Mx+M^{x+} ions in saturated solution,
    • [Xm]x\left[\mathrm X^{m-}\right]^x - molar concentration of Xm+X^{m+} ions in saturated solution.
  • The solubility equilibrium is measured for saturated solution.
  • The solubility equilibrium is specific for a given substance.
  • Alternative name for solubility equilibrium is solubility product constant.
  • The solubility equilibrium is varies depending on the temperature. Chemical tables most often give values for 298K (25°C).
  • If product of ion concentrations in real solution exceeds the value of solubility equilibrium then it forms the precipitate.
  • If we know the solubility equilibrium and dissociation reaction, then we can calculate molar solubility of substance:
    S=Kspxxmmx+mS = \sqrt[x+m]{\dfrac{K_{sp}}{x^{x} m^{m}}}
    where:
    • SS - molar solubility of substance MmXxM_mX_x,
    • KspK_{sp} - solubility equilibrium,
    • xx - stoichiometric coefficient determined by dissociation reaction (see above),
    • mm - stoichiometric coefficient determined by dissociation reaction (see above).

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