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

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# hydroxides#

 Substance Molecular formula Solubility equilibrium yttrium (III) hydroxide Y(OH)3 1×10-22 zinc hydroxide Zn(OH)2 3×10-17 thallium (III) hydroxide Tl(OH)3 1.68×10-44 scandium hydroxide Sc(OH)3 2.22×10-31 tin (II) hydroxide Sn(OH)2 5.45×10-27 lead (II) hydroxide Pb(OH)2 1.43×10-20 nickel hydroxide Ni(OH)2 5.48×10-16 magnesium hydroxide Mg(OH)2 5.61×10-12 copper (II) hydroxide Cu(OH)2 1.99×10-20 cobalt (II) hydroxide Co(OH)2 5.92×10-15 cadmium (II) hydroxide Cd(OH)2 7.2×10-15 calcium hydroxide Ca(OH)2 0.00000502 beryllium hydroxide Be(OH)2 6.92×10-22 barium hydroxide octahydrate Ba(OH)2 · 8H2O 0.000255 iron (II) hydroxide Fe(OH)2 4.87×10-17 iron (III) hydroxide Fe(OH)3 2.79×10-39 aluminium hydroxide Al(OH)3 5×10-33 silver (I) hydroxide AgOH 1.5×10-8

# Some facts#

• If the substance $M_mX_x$ dissociates in the solution according to the reaction:
$M_mX_x \iff m M^{x+} + x X^{m-}$
then its solubility equilibrium is defined as below:
$K_{sp} = \left[\mathrm M^{x+}\right]^m \left[\mathrm X^{m-}\right]^x$

where:
• $K_{sp}$ - solubility quilibrium of substance,
• $\left[\mathrm M^{x+}\right]^m$ - molar concentration of $M^{x+}$ ions in saturated solution,
• $\left[\mathrm X^{m-}\right]^x$ - molar concentration of $X^{m+}$ 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:
$S = \sqrt[x+m]{\dfrac{K_{sp}}{x^{x} m^{m}}}$
where:
• $S$ - molar solubility of substance $M_mX_x$,
• $K_{sp}$ - solubility equilibrium,
• $x$ - stoichiometric coefficient determined by dissociation reaction (see above),
• $m$ - stoichiometric coefficient determined by dissociation reaction (see above).

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