https://doi.org/10.1351/goldbook.15358
Solubility of a diatomic gas in a molten metal is proportional to the square root of the partial pressure.
Notes:
- The law follows from the solubility constant for equilibrium dissolution of an ideal diatomic gas \(\ce{X2}\) in a metal \(\ce{M}\) to form an ideal solution of dissociated atoms: \[\ce{X2(g) <=> 2X(M)}\] for which, and for dilute solutions of the gas, \[K_{{\rm{s}},x} = a(\ce{X},\ce{M})^{2}/a(\ce{X2},{\rm{g}}) \approx x(\ce{X},\ce{M})^{2} p^{_{^⦵\!}}/p (\ce{X2},\rm{g})\] where \(x(\ce{X},\ce{M})\) is the solubility of the gas in the molten metal expressed as a mole fraction of \(\ce{H\mbox{-}atoms}\). The solubility constant \(K_{\rm{s},x}\) is called the Sieverts constant.
- Other forms of the solubility constant are common, especially in terms of amount concentrations or mass fractions (especially in metallurgical papers) instead of mole fractions.
See also: solubility constant