By Henry’s Law, the concentration of a dissolving gas in a liquid is proportional to the partial pressure of that gas in contact with the liquid, mathematically, $ p = k_\mathrm{H} c$, where $p$ is the partial pressure of the dissolving gas, $c$ is the concentration of the dissolving gas in the liquid (solution), and $k_\mathrm{H}$ is a constant (Henry’s constant?) which depends on temperature.

What is the value of $k_\mathrm{H}$ for common noble gases (in particular, xenon) in concentrated phosphoric acid, at, say $298~\mathrm{K}$? Can the solubility at other temperatures be calculated using an extrapolation formula?


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Value seems to be $k_H^{\ominus}=4.3\times10^{-3}\;M/atm$ for Xenon in water.For it in conc. phosporic acid seems not to be available as probably no one has carried the experiment in this solvent since water is most common and used commonly.Maybe you would?

Also, A simple way to describe Henry’s law as a function of temperature is: $$\LARGE k_H=k_H^{\ominus}\times e^{\left(\frac{-\Delta_{soln}H}R\left(\frac1T-\frac1{T^{\ominus}}\right)\right)}$$ where $\Delta_{soln}H=$enthalpy of solution. Here, the temperature dependence is: $$\frac{-d\ln k_H}{d(1/T)}=\frac{\Delta_{soln}H}R$$

Useful Links: Table of constants, The NIST Chemistry WebBook, The Pesticide Properties Database (PPD)


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